A  DICTIONARY  OF  CHEMICAL  SOLUBILITIES 


INORGANIC 


THE  MACMILLAN  COMPANY 

NEW  YORK  •  BOSTON  •  CHICAGO  •  DALLAS 

'ATLANTA  •  SAN  "FRANCISCO 

MACMILLAN  &  CO.,  LIMITED 

LONDON   •  BOMBAY   •  CALCUTTA 
MELBOURNE 

THE  MACMILLAN  CO.  OF  CANADA,  LTD 

TORONTO 


DICTIONARY 

OF 

CHEMICAL  SOLUBILITIES 

INORGANIC 

FIRST  EDITION 

BY 

ARTHUR  MESSINGER  COMEY,  PH.D. 

//    * 

SECOND  EDITION 

ENLARGED    AND    REVISED 
BY 

ARTHUR  MESSINGER  COMEY,  Pn.D. 

DIRECTOR,   EASTERN  LABORATORY,   E.   I.  DU  PONT  DE    NEMOURS  AND  CO. 

AND 

DOROTHY  A.  HAHN,  PH.D. 

PROFESSOR  OF  CHEMISTRY,   MT.   HOLYOKE   COLLEGE 


THE  MACMILLAN  COMPANY 
1921 

Att  rights  reserved 


/ii 


'*/ 

•MIMINCt   O«.I"T( 


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COPYRIGHT,  1921 

MACMILLAN  COMPANY 


Set  up  and  printed  Published  February,  1921 


PREFACE  TO  FIRST  EDITION 

FOE  many  years  a  need  has  been  felt  by  chemists  for  a  book  which  shall  collect 
into  convenient  form  for  ready  reference  the  various  data  concerning  the  solu- 
bility of  chemical  substances  that  have  been  published  from  time  to  time  in 
chemical  periodicals  and  elsewhere. 

The  first  mention  that  can  be  found  of  such  a  plan  was  made  in  1731,  when 
Peter  Shaw  delivered  Chemical  Lectures  in  London,  as  may  be  seen  from  the 
following: — 

EXTRACTS  from  PETER  SHAW'S  Chemical  Lectures,  publickly  read  at  London  in 
1731  and  1732.    London.    Second  Edition,  London  1755.    8vo. 

Page  97.  Experiment  I. — That  Water  as  a  Menstruum  dissolves  more  of  one  body 
and  less  of  another. 

[He  shows  that  two  ounces  of  water  dissolve  two  ounces  of  Epsom  salt,  five  drachms  of 
common  salt,  and  eight  grains  of  cream  of  tartar.  Only  in  the  latter  case  much  remained 
undissolved  until  boiled.] 

"It  might  be  proper  for  the  further  Improvement  of  Chemistry  and  Natural  Phi- 
losophy to  form  a  Table  of  the  Time  and  Quantity  wherein  all  the  known  Salts  are 
dissolvable  in  Water.  .  .  .  Such  a  Table  regularly  formed  might  ease  the  Trouble  of  re- 
fining Salts,  by  shewing  at  once  without  future  Trial  or  Loss  of  Time  how  much  Water 
each  Salt  required  to  dissolve  it  for  Clarification,  Filtration,  or  Crystallization.  It  would 
likewise  supply  us  with  a  ready  and  commodious  Way  of  separating  any  Mixture  of  Salts, 
by  shewing  which  would  first  shoot  out  of  the  Mixture  upon  Crystallization.  .  .  .  The 
same  Table  might  also  direct  us  to  a  ready  and  commodious  Method  of  separating  two 
Salts  without  waiting  for  Crystallization.  .  .  ." 

It  was  many  years,  however,  before  the  scheme  suggested  by  Peter  Shaw 
was  put  into  execution.  Professor  F.  H.  Storer  published  the  first  work  that 
undertook  to  carry  out  the  idea  in  its  entirety,  in  1864,  in  a  book,  which  he 
entitled  "  First  Outlines  of  a  Dictionary  of  Solubilities  of  Chemical  Substances," 
and  which  contained  a  compilation  of  nearly  all  the  data  on  the  subject  pub- 
lished before  1860.  It  was  at  once  recognized  as  a  most  valuable  contribution 
to  chemical  literature;  but  for  many  years  it  has  been  difficult  to  obtain  this 
work,  as  the  limited  edition  which  was  published  was  soon  wholly  exhausted. 
Since  then  nothing  has  appeared  on  the  subject  except  the  brief  tabulations 
found  in  various  reference  books,  and  no  attempt  has  been  made  to  cover  the 
whole  subject. 

It  is  needless  to  state  that  the  growth  of  chemical  science  since  the  publication 
of  Professor  Storer's  book  has  been  so  enormous  that  that  work  has  lost,  at  least 
to  a  great  extent,  the  practical  value  it  possessed  thirty  years  ago.  This  growth 
has  been  indeed  so  great,  and  the  data  which  have  accumulated  since  1860  so  far 
surpass  the  earlier  in  volume,  that  a  simple  revision  of  Professor  Storer's  book 
was  impracticable,  and  it  therefore  seemed  best  to  start  afresh. 

A  o  A  rr  *r  tr 


vi  PREFACE   TO   FIRST  EDITION 

With  the  facilities  offered  by  the  various  scientific  libraries  at  Harvard 
University,  the  Massachusetts  Institute  of  Technology,  and  other  libraries  in 
Boston,  it  has  been  possible  to  collect  nearly  all  the  data  relating  to  the  subject. 
For  the  work  before  1860  Professor  Storer's  work  has  been  found  invaluable.  | 

The  method  pursued  has  been  to  form  a  preliminary  list  of  compounds 
with  more  or  less  data  by  consulting  the  two  most  complete  works  on  inorganic 
chemistry — Gmelin-Kraut's  "Handbuch  der  anorganischen  Chemie"  and 
Graham-Otto-Michaelis's  "Lehrbuch."  These  statements  have  been  verified 
and  elaborated  by  consulting  the  original  memoirs  in  all  the  periodicals  devoted 
to  chemical  literature  which  were  obtainable.  The  ' '  Jahresbericht  der  Chemie ' ' 
also  has  been  used  extensively  in  tracing  references,  but  the  original  memoirs 
have  always  been  consulted  and  references  given  to  them  when  possible. 

It  has  been  found  impracticable  to  draw  any  distinction  as  to  reliability 
between  the  various  data  given  by  different  observers.  It  was  manifestly 
impossible  to  attempt  to  verify  experimentally  the  statements  of  those  who 
have  carried  on  the  researches,  for  the  most  assiduous  labor  of  many  could 
only  cover  a  small  portion  of  the  attested  facts.  Therefore,  even  when  two 
statements  are  directly  contradictory,  both  have  been  given  with  the  authority 
for  each.  The  only  exception  to  this  has  been  made  when  more  recent  dis- 
coveries have  shown  beyond  any  reasonable  doubt  the  falsity  of  previous  work. 
In  this  way  some  of  the  older  manifestly  inaccurate  work  has  been  omitted.  In 
a  majority  of  cases  the  more  recent  work  may  be  considered  to  be  the  more 
accurate,  but  this  is  not  the  invariable  rule.  A  Synchronistic  Table  of  the  more 
common  periodicals  is  given  in  the  Appendix,  whereby  it  is  easy  to  determine 
the  date  of  the  publication  of  a  research  to  which  reference  is  made. 

It  may  be  objected  by  the  practical  chemist  that  most  of  the  work  previous 
to  1850  might  well  have  been  omitted,  but  a  great  deal  of  this  work  possesses  at 
least  a  historical  -value,  and  often  furnishes  facts  which  have  not  since  been 
verified.  Much  of  the  earlier  work,  when  obviously  of  less  importance,  has  been 
printed  in  smaller  type. 

The  aim  has  been  to  include  in  this  volume  all  analyzed  inorganic  substances, 
that  is,  all  substances  which  do  not  contain  carbon,  but  exception  has  been  made 
in  the  case  of  CO2,  CO,  C$2,  the  carbonates,  cyanides,  ferro-cyanides,  etc., 
which  are  here  included. 

The  work  has  been  brought  up  to  March,  1894,  when  this  volume  went  to 
press,  and  the  results  of  researches  published  since  that  time  are  not  included 
in  the  present  edition. 

It  is  hoped  that  this  book  will  fill  to  some  extent  the  want  that  has  been  felt 
by  chemists  for  a  compilation  of  this  nature.  While  it  has  been  attempted  to 
make  the  book  as  free  from  errors  as  possible,  nevertheless  it  is  naturally  im- 
possible to  avoid  many  mistakes,  and  the  compiler  will  be  very  grateful  to  those 
who  may  call  his  attention  to  any  errors  or  omissions. 

A.  M.  C. 
CAMBRIDGE,  MASS.,  Aug.,  1895. 


PREFACE  TO  SECOND  EDITION 

DURING  the  twenty-five  years  which  have  elapsed  since  the  publication  of  th< 
first  edition  of  this  dictionary,  a  very  large  amount  of  work  has  been  publishe( 
in  chemical  periodicals,  containing  data  concerning  the  solubility  of  inorgani 
chemical  compounds.  As  it  was  impossible  for  the  compiler  of  the  first  editioi 
to  devote  the  time  necessary  for  the  collecting  of  the  published  data,  it  wa 
necessary  to  employ  assistance,  and  Dr.  Dorothy  A.  Hahn,  Professor  of  Chem 
istry,  Mt.  Holyoke  College,  was  engaged  for  this  work.  Dr.  Hahn  has  collectec 
the  larger  part  of  the  material  in  this  book,  which  work  in  spite  of  its  arduou 
and  tedious  nature,  she  has  performed  in  a  most  painstaking  manner. 

The  compilation  and  arrangement  of  the  data  collected  by  Dr.  Hahn,  whicl 
devolved  upon  the  original  author,  took  much  time.  This,  together  with  diffi 
culties  in  printing,  caused  by  the  general  conditions  after  the  war,  has  delaye( 
the  publication  until  the  present  year,  although  the  work  was  begun  in  1916 
and  it  has  only  been  brought  up  to  January  1st  of  that  year. 

Since  the  publication  of  the  first  edition  of  this  work,  Dr.  Atherton  Seidell  ha: 
brought  out  two  editions  of  his  book,  entitled  "  Solubilities  of  Inorganic  anc 
Organic  Substances,"  which  covers  quite  a  different  field,  as  he  considers  onb 
quantitative  data  and  those  only  for  the  commoner  substances.  Dr.  Seidell  hai 
followed  the  plan  in  most  cases  where  there  are  several  available  solubility 
determinations  of  a  substance,  of  selecting  and  averaging  the  more  reliabli 
results,  and  embodying  them  in  tables.  Although  this  undoubtedly  facilitate 
ready  reference,  it  has  seemed  better  to  adhere  to  the  original  plan  of  the  firs 
edition,  and  to  publish  all  the  data  in  the  form  of  the  original  authorities  witl 
references  and  dates,  so  that  the  user  may  be  at  liberty  to  use  his  own  judgmen 
in  selection.  Some  few  of  the  tables  arranged  by  Dr.  Seidell,  however,  hav< 
seemed  to  possess  decided  advantages  over  any  other  published  data  and  the;; 
have  been  incorporated  in  the  present  volume.  It  is  desired  also  to  acknowledg< 
indebtedness  to  Dr.  Seidell's  work  for  certain  other  tables  where  the  origina 
sources  were  not  available  to  the  present  compilers. 

The  same  plan  and  arrangement  used  in  the  first  edition  has  been  followec 
with  certain  elaboration,  however,  of  the  arrangement  of  data  on  the  solubility 
of  two  or  more  salts  in  a  solvent,  which  is  explained  in  the  Explanatory  Preface 

Data  published  since  the  first  edition  on  the  cobalt  and  chromium  ammonh 
compounds  and  those  of  the  platinum  group  have  been  omitted,  as  it  seemec 
that  solubility  data  on  those  compounds  possessed  very  little  general  interest. 

As  stated  in  the  preface  of  the  first  edition,  while  every  possible  attempt  hai 
been  made  to  avoid  errors,  it  is  manifestly  impossible  to  avoid  many  mistakes  ii 
a  work  of  this  nature,  and  the  compiler  will  be  glad  to  have  his  attention  callec 
to  any  errors  or  omissions. 

WILMINGTON,  Del.,  Jan.,  1921.  A.  M.  C. 


EXPLANATORY  PREFACE 

IN  order  to  reduce  this  volume  to  a  convenient  size  the  subject-matter  has  been 
abbreviated  and  condensed  as  far  as  seemed  compatible  with  clearness;  but  it 
has  been  the  aim  not  to  use  any  abbreviations  which  are  not  at  once  intelligible 
without  consulting  the  explanatory  table.  The  more  common  chemical  for- 
mulae have  been  universally  used,  thereby  saving  a  large  amount  of  space 
without  detracting  from  ready  intelligibility  to  chemists. 

The  solubility  of  the  substance  in  water  is  first  given,  the  data  being  arranged 
chronologically  in  the  longer  articles.  Then  follow  the  specific  gravities  of  the 
aqueous  solutions,  and  also  any  data  obtainable  regarding  their  boiling-points; 
other  physical  data  concerning  solutions  are  not  included.  Following  this  is  the 
solubility  of  the  substance  in  other  solvents — first  the  inorganic  acids,  then 
alkali  and  salt  solutions,  and  finally  organic  substances. 

Owing  to  the  great  increase  of  data,  published  during  the  last  twenty  years, 
on  the  simultaneous  solubility  of  two  or  more  salts  in  a  given  solvent,'  it  has 
been  found  necessary  to  plan  some  arrangement,  whereby  such  data  can  easily 
be  found,  and  the  plan  adopted  is  as  follows:  The  data  for  the  solubility  of  two 
salts  in  a  solvent  is  placed  under  the  salt  which  comes  first  according  to  the 
alphabetical  arrangement  in  this  dictionary,  and  the  order  of  the  data  on  various 
salts  under  the  same  heading  follows  the  alphabetical  order  of  the  salts  consid- 
ered. Thus  the  data  on  the  solubility  of  NH4Cl+BaCl2,  NH4Cl+CuCl2, 
and  NH4ClH-PbCl2,  and  NH^Cl-HNEU^SCX  are  placed  under  Ammonium 
Chloride  and  arranged  in  the  given  order.  Certain  exceptions  have  been  made 
to  this  rule,  where  the  data  directly  concerns  the  solubility  of  a  salt  in  a  solu- 
tion of  another  salt,  in  which  case,  it  is  placed  under  the  former.  Numerous 
cross  references,  however,  are  given,  which  it  is  hoped  will  avoid  confusion. 

In  many  cases  no  definite  distinction  can  be  drawn  between  the  phenomena 
of  solution  and  decomposition.  At  present  the  theory  of  solution  is  in  a  confused 
state,  and  until  what  really  takes  place  when  a  substance  dissolves  is  thoroughly 
understood  no  distinct  line  can  be  drawn.  The  whole  subject  is  unsettled  at  the 
present  time;  for  while  many  chemists  believe  in  the  so-called  "dissociation" 
theory,  yet  the  "hydrate"  theory  is  not  without  its  supporters.  It  is  not  my 
intention  to  discuss  the  theoretical  side  of  the  question,  which  has  been  so  well 
treated  in  many  recent  works.  It  is,  however,  obvious  that  the  phenomena  are 
essentially  different,  when,  for  example,  sodium  carbonate  is  dissolved  in  water, 
in  which  case  the  original  salt  is  deposited  on  evaporation,  and  when  iron  is 
dissolved  in  sulphuric  acid,  and  the  solution  deposits  a  sulphate  of  iron.  Yet  it 
is  still  the  custom  to  speak  of  iron  as  soluble  in  sulphuric  acid,  although  it  would 
be  much  more  accurate  to  say  that  the  sulphuric  acid  was  decomposed  by  the 
iron.  It  has  thus  been  found  impracticable  to  draw  a  sharp  line  between  solu- 


EXPLANATORY  PREFACE 


tion  and  decomposition,  and  the  term  "  soluble  "  has  in  general  been  used 
where  a  solution  of  some  sort  is  formed  by  the  action  of  the  solvent. 

The  matter  of  alphabetical  arrangement  of  chemical  compounds,  in  the 
present  somewhat  confused  state  of  chemical  nomenclature,  has  been  a  difficult 
question  to  decide.  The  plan  followed  has  been  practically  that  of  the  standard 
Dictionaries  of  Chemistry,  whereby  the  compounds  of  metals  with  one  of  the 
non-metallic  elements  have  been  classified  under  the  metals,  while  the  salts  of 
the  other  acids  (the  oxygen  acids  so  called  and  some  few  others)  have  been 
arranged  alphabetically  under  the  acids.  Thus  barium  chloride  is  found  under 
barium,  while  barium  chlorate  is  found  under  chloric  acid.  No  exception  has 
been  made  in  the  case  of  the  rare  metals,  as  is  usually  the  custom  in  Dictionaries 
of  Chemistry.  Double  salts  are  to  be  found  under  the  word  which  comes  first 
alphabetically;  thus,  " common  alum,"  potassium  aluminum  sulphate,  is  found 
under  aluminum  sulphate  as  aluminum  potassium  sulphate  (under  sulphuric 
acid),  but  ammonia  chrome  alum  is  found  under  ammonium  sulphate  as  am- 
monium chromium  sulphate.  In  the  same  way  the  double  sulphate  and  chro- 
mate  of  potassium  is  found  under  potassium  chromate  (chromic  acid),  and  not 
under  potassium  sulphate  (sulphuric  acid) .  The  double  chloride  of  ammonium 
and  magnesium  is  found  under  ammonium  chloride  (ammonium),  while  the 
double  chloride  of  potassium  and  magnesium  is  found  under  magnesium  chloride 
(magnesium).  An  exception  is  made,  however,  in  the  case  of  double  compounds 
of  salts  of  oxygen  acids  with  salts  containing  a  single  non-metallic  element,  in 
which  case  they  are  always  found  under  the  oxygen  acid.  Thus  the  double 
sulphate  and  chloride  of  lead,  PbSO4,  PbC^,  is  found  under  lead  sulphate 
(sulphuric  acid),  and  not  under  lead  chloride  (lead). 

The  above  method  in  some  cases  widely  separates  analogous  compounds, 
but  it  was  found  to  be  the  only  practical  way  to  a  strictly  alphabetical  arrange- 
ment, which  is  no  necessary  in  a  book  containing  so  many  very  short  articles. 

The  ammonia  addition-products  furnished  another. difficulty.  While  their 
nature  is  more  or  less  definitely  understood  in  the  cobalt,  platinum,  etc.,  com- 
pounds, and  a  definite  nomenclature  is  in  general  use,  there  is  an  absolute  lack 
of  anything  of  the  kind  in  the  less  definite  compounds.  It  is  good  usage  to 
speak  of  cuprammonium  compounds,  but  how  shall  we  designate  the  analogous 
cadmium  compounds?  "  Cadmammonium  "  has  not 'yet  received  the  sanction 
of  chemists,  and  A1C13,  NH3  is  a  still  worse  case  for  naming.  I  have,  therefore, 
not  attempted  to  name  these  compounds,  but  classified  them  all  under  the  salts 
to  which  the  ammonia  is  added,  affixing  the  word  ammonia,  thus:  aluminum 
chloride  ammonia,  cadmium  chloride  ammonia,  and  also  cupric  chloride  am- 
monia for  the  salt  now  almost  universally  known  as  cuprammonium  chloride. 

The  ammonia  compounds  of  cobalt,  chromium,  mercury,  and  the  platinum 
metals  are  arranged  alphabetically  according  to  their  universally  accepted 
names,  a  list  of  which  i,s  given  under  each  of  those  elements. 

It  has  further  been  necessary  to  settle  arbitrarily  the  question  whether  a  sub- 
stance should  be  considered  as  a  double  salt  or  a  salt  of  a  compound  acid  con- 


EXPLANATORY  PREFACE  xi 

taining  one  of  the  metals.  For  example,  "  fluosilicates "  (or  silicofluorides,  as 
some  may  prefer)  is  the  general  name  for  the  double  fluorides  of  SiF4  and  a 
metal,  but  this  unanimity  in  usage  gradually  disappears  as  the  basic  elements 
become  more  nearly  alike,  so  that  it  is  impossible  to  draw  a  line  between  such 
compounds  and  a  compound  such  as  the  double  chloride  of  magnesium  and 
potassium,  for  which  indeed  the  name  "potassium  chloromagnesate "  has  been 
proposed.  The  aim  has  been  in  all  these  cases  to  follow  the  best  usage  rather 
than  make  an  absolutely  homogeneous  system  of  nomenclature  out  of  the  exist- 
ing confusion. 

In  the  matter  of  formulae  no  attempt  at  uniformity  has  been  made.  Thus  in 
the  case  above  some  chemists  write  the  formula  of  the  double  chloride  of  mag- 
nesium and  potassium  as  KMgCl3,  others  as  KC1,  MgCl3.  The  form  here 
used  has  been  in  most  cases  that  of  the  author  from  whom  the  data  are  taken. 

The  prefixes  mono,  di,  tri,  ortho,  pyro,  etc.,  have  in  general  been  disregarded 
in  the  alphabetical  arrangement,  and  have  been  printed  in  italics.  Exceptions 
to  this  have  been  made,  however,  in  the  cobalt,  chromium,  etc.,  ammonium 
compounds,  and  in  a  few  others,  as  dithionic,  perchloric,  etc.,  acids.  Cross 
references  have  been  used,  so  as  to  prevent  any  confusion  arising  from  lack  of 
uniformity  in  this  respect. 

In  the  Appendix  will  be  found  formulae  and  tables  for  the  conversion  of  the 
degrees  of  various  hydrometer  scales  into  specific  gravity,  and  a  Synchronistic 
Table  of  the  Periodicals  to  which  references  are  most  frequently  made. 


ABBREVIATIONS 


abs . — absolute . 

atmos . — atmosphere . 

b.-pt. — boiling-point. 

comp . — compound. 

cone . — concen  trated . 

corr. — corrected. 

cryst. — crystallised,  crystalline 

decomp. — decompose,   decomposes, 

decomposition,  etc. 
dil. — dilute, 
eutec. — eutectic. 
insol . — insoluble . 
M. — a  univalent  Metal. 
M  in . — M  ineral . 
mol. — molecule. 


m.-pt. — melting-point, 
ord. — ordinary, 
n. — normal. 

ppt.,  pptd.,  etc. — precipitate,  pre- 
cipitated, etc. 
pt. — part, 
sat. — saturated, 
si. — slightly, 
sol. — soluble, 
sp.  gr. — specific  gravity, 
supersat. — supersaturated. 
t°  =  temperature  in  Centigrade  degrees, 
temp. — temperature, 
tr.  pt. — transition  point, 
vol. — volume. 


ABBREVIATIONS  OF  REFERENCES 

A.— Annalen  der  Pharmacie,  edited  by  Liebig  and  others,  1832-39;  continued  as  Annalen  der 
Chemie  und  Pharmacie,  1840-73;  continued  as  Justus  Liebig's  Annalen  der  Chemie, 

A.  ch. — Annales  de  Chimie  et  de  Physique.  Paris.  1st  series,  1789-1816,  96  vols  ;  2nd 
series,  1817-40,  78  vols.;  3rd  series,  1841-63,  69  vols.;  4th  series,  1864-73,  30  vols.; 
5th series,  1874-83, 30  vols.;  6th series,  1884-93, 30  vols.: 7th series,  1893-1903, 30  vols  ; 
8th  series,  190^13,  30  vols.;  9th  series,  1914 +,  3  vols. 

Acta  Lund. — Acta  Universitatis  Lundensis/or  Lunds  Universitets  Ars-skrift.   Lund   1864+ 

Am.  Chemist. — The  American  Chemist.    New  York,  1870-77.    7  vols. 

Am.  Ch.  J. — The  American  Chemical  Journal,  edited  by  Remsen.  Baltimore,  187&-1913 
50  vols. 

Am.  J.  Sci. — American  Journal  of  Science  and  Arts,  edited  by  Silliman,  Dana,  and  others. 
New  Haven.  1st  series,  1818-45,  50  vols.;  2nd  series,  1846-70,  50  vols.;  3rd  series, 
1871-95,  50  vols.;  4th  series,  1896-1915 +,  40  vols.  Also  numbered  consecutively,  190 
vols. 

Analyst.— The  Analyst.    London,  1876-19 15+.    45  vols. 

Ann.  chim.  farm. — Annali  di  chimica  e  di  farmacologia.    Milan,  1886-90.    5  vols. 

Ann.  des  Mines. — See  Ann.  Min. 

Ann.  Min. — Annales  des  Mines.     Paris. 

Ann.  Phil. — Annals  of  Philosophy.  London.  1st  series,  1813-20,  16  vols.;  new  series, 
1821-26,  12  vols. 

Ann.  Phys. — See  Pogg.  and  W.  Ann. 

Apoth.  Z. — Apotheker-Zeitung.     Berlin. 

Arb.  Kais.  Gesundheitsamt. — Arbeiten  aus  dem  Kaiserlichen  Gesundheitsamte. 

Arch.  Ne'er.  Sc. — Archives  Ne"erlandaises  des  Sciences  exactes  et  naturelles. 

Arch.  Pharm. — Archiv  der  Pharmacie,  continued  from  Archiv  des  Apothekervereins  in 
Norddeutschland,  which  forms  the  1st  series.  1st  series,  1822-34,  50  vols.;  2nd  series, 
1835-72,  150  vols.;  3rd  series,  1873-94+,  32  vols.  Also  numbered  consecutively, 
which  system  is  exclusively  used  after  3rd  series,  vol.  253  (1915). 

Arch.  sc.  Phys.  nat. — Archives  des  sciences  physiques  et  naturelles  de  la  Bibliotheque 
universelle  de  Geneve. 

A.  Suppl. — Annalen  der  Chemie  und  Pharmacie.    Supplement-Bande.    Vol.  i.  1861;  vol.  ii, 

1862-63;  vol.  iii.  1864-65;  vol.  iv.  1865-66;  vol.  v.  1867;  vol.  vi.  1868;  vol.  vii.  1870; 

vol.  viii.  1872. 

B—  Berichte  der  deutschen  chemischen  Gesellschaft.    Berlin,  1868-1915+.  48    vols. 
Att.  Ace.  Line. — Atti  della  reale  accademia  dei  Lincei,  rendconditi,  etc. 

B.  A.  B. — Sitzungsberichte  der  koniglichen  preussischen  Akademie  der  Wissenschaften  zu 

Berlin. 

Belg.  Acad.  Bull. — Bulletin  de  1' Academic  Royale  des  Sciences,  des  Lettres,  et  des  Beaux- 
Arts  de  Belgique. 

Berz.  J.  B. — Jahresbericht  iiber  die  Fortschritte  der  physischen  Wissenschaften,  edited  by 
Berzelius.  1822-47.  30  vols. 

Br.  Arch. — Archiv  des  Apothekervereins  im  nordlichen  Teutschland,  etc.,  edited  by  Brandes. 
1st  series,  1822-31,  39  vols.,  corresponds  to  1st  series  of  Arch.  Pharm. 

Bull.  A.cad.  Crac. — Bulletin  international  de  I'Acad&nie  des  Sciences  de  Cracovie. 

Bull.  Ac.  St.  Petersb. — Bulletin  de  1' Academic  Impe"riale  des  Sciences  de  St.  Pe"tersbourg. 

Bull.  Soc.— Bulletin  des  Stances  de  la  Socie'te'  chimique  de  Paris.  2nd  series,  1864-88,  50 
vols.:  3rd  series,  1889-1906,  36  vols.;  4th  series,  1907-15+,  18  vols. 

Bull.  Soc.  chim.  Belg. — Bulletin  de  la  Socie"te"  chimique  Belgique. 

Bull.  Soc.  ind.  Mulhouse.—  Bulletin  de  la  Soci6t<§  industrielle  de  Mulhouse.    1828-49.    22  vols. 

Bull.  Soc.  Min. — Bulletin  de  la  socifte"  franchise  de  Mine'ralogie.    1878-1915+.    37  vols. 

C.  A. — Chemical  Abstracts.    American  Chemical  Society.    New  York. 

C.   C. — Chemisches   Centralblatt,   continued  from   Pharmaceutisches  Centralblatt. 

C.  B.  Miner. — Centralblatt  fur  mineralogie,  Geologic  und  Palseontologie.    Berlin. 

Chem.  Ind. — Die  Chemische  Industrie,  edited  by  Jacobsen.    Berlin. 

Chem.  Soc. — Journal  of  the  Chemical  Society  of  London.      1st  series,  1849-62,  15  vols.;  2nd 

series,  1863-78, 17  vols. ;  new  series,  1878-19 15+.  The  vols.  are  numbered  consecutively 

from  1849.   1878  =  vol.  32.   Total,  108  vols. 


xvi  ABBREVIATIONS  OF  REFERENCES 

Chem.-tech.  Centr-Anz. — Chemisch-technischer  Central- Anzeiger.  « 

Chem.  Weekbl. — Chemiker  Weekblad. 

Chem.  Z.— See  Ch.  Z. 

Chem.  Zeitschr. — Chemische  Zeitschrift. 

Ch.  Gaz. — The  Chemical  Gazette.    London,  1843-59.    17  vols. 

Ch.  Kal. — Chemiker  Kalender,  edited 'by  Biedermann. 

Ch.  Z. — Chemiker  Zeitung. 

Ch.  Z.  Repert  —  Chemisches  Repertorium  Beiblatt  zur  Chemiker-Zeitung.    Gothen. 

Cim.— II  Cimento.    Turin,  1852-54.    6  vols. 

C.  N. — The  Chemical  News.    London;  1860-1915 +.  112   vols. 

Comm. — Commentar  zur  Pharmacopoea  germanica  by  Hager.    Berlhi,  1883. 

Compt.  chim. — Comptes-rendus  mensuels  des  Travaux  chimiques,  edited  by  Laurent  and 

Gerhardt.     1845-51.     7  vols. 
C.  R. — Comptes-rendus  hebdomadaires  des  Seances   de    1' Academic  des  Sciences.     Paris, 

1835-19 15+.     161  vols. 
Crell.  Ann. — Chemische  Annalen  fur  die  Freunde-  der  Naturlehre,  etc.,  edited  by  Crell. 

1784-1803.     40  vols. 
Dansk.  Vid.  For. — Oversigt  over  det  kgl.  danske    Videnskabernes  Selskabs  Forhandlinger. 

Copenhagen. 
Dingl. — Dingler's  Polytechnisches  Journal,  edited  by  Dingier  and  others.    1820-1915+ . 

330  vols. 

Edinb.  Trans.— Transactions  of  the  Royal  Society  of  Edinburgh.     1788-1915+ .     51  vols. 
Ed.  J.  Sci. — The  Edinburgh  Journal  of  Science.      1st  series,  1824-29,  10  vols.;  2nd  series, 

1829-32,  6  vols.    Continued  as  Phil.  Mag. 

Electrochem.  Ind. — Electrochemical  Industry   (Oct.,   1902,  to  Dec.,   1904)  later  Electro- 
chemical and  Metallurgical  Industry.    New  York. 
Elektrochem  Z. — Elektrochemische  Zeitschrift.     Berlin. 
Eng.  Min.  J. — The  Engineering  and  Mining  Journal.    New  York. 
Gazz.  ch.  it. — Gazzeta  chimica  italiana.    Palermo,  1871-1915+.    45  vols. 
Gilb.  Ann.— Annalen  der  Physik,  edited  by  Gilbert.      1st  series,  1799-1808,  30  vols.;  2nd 

series,  1809-18,  30  vols.;  3rd  series.,  1819-24,  26  vols.     Also  numbered  consecutively. 

76  vols.     Continued  as  Pogg. 
Gm.-K. — Gmelin-Kraut's  Handbuch  der  anorganischen  Chemie,  6te  Auflage.    1877-1905. 

7te  Auflage,  1907-1915+. 
Gr.-Ot. — Graham-Otto's  ausfiihrliches  Lehrbuch  der  anorganischen  Chemie,  5te  Auflage,  by 

Michaelis.     1878-89. 
Jahrb.  Miner. — Jahrbuch  fur  Mineralogie,  Geologic  und  Palseontologie.    Heidelberg.    1830- 

1832.    Then.     Neues  Jahrbuch  fur  Minerologie.    Stuttgart. 
Jahrb.  d.  Pharm. — Jahresbericht  der  Pharmacie. 
J.  Am.  Chem.  Soc. — Journal  of  the  American  Chemical  Society.    New  York,  1876-1915+. 

37  vols. 
J.  Anal.  Appl.  Ch. — The  Journal  of  Analytical  and  Applied  Chemistry,  edited  by  Hart. 

1887-93.     7  vols. 

J.  B. — Jahresbericht  iiber  die  Fortschritte  der  Chemie,  u.  s.  w. 
J.  Chim.  me"d. — Journal  de  Chimie  medicale,  de  Pharmacie,  et  de  Toxicologie.     1st  series, 

1825-34,  10  vols.;  2nd  series,   1835-44,    10  vols.;  3rd  series,   1845-54,  10  vols.;  4th 

series,  1855-64,  10  vols.;  5th  series;  1865-76.     12  vols. 
Jena.  Zeit. — Jenaische  Zeitschrift  fur  Medicin  und  Naturwissenschaften. 
J.  Pharm. — Journal  de  Pharmacie  et  de  Chimie.     Paris.     2nd  series,  1815-41,  27  vols.;  3rd 

series,  1842-64,  46  vols.;  4th  series,  1865-79,  30  vols.;  5th  series,  1879-94:  6th  series, 

1895-1909,  30  vols.;  7th  series,  1910-15+,  10  vols. 

J.  Phys:— Journal  der  Physik,  edited  by  Gren.    1790-98.    12  vols.    Continued  as  Gilb  Ann 
J.  Phys.  Ch.— The  Journal  of  Physical  Chemistry.    Ithaca,  N.  Y. 
J.  pr. — Journal  fur  praktische  Chemie,  edited  by  Erdmanix,  Kolbe,  and  v.  Meyer.    Leipzig 

1st  series,  1834-69,  108  vols.;  2nd  series,  1870-1915  +  .   92  vols. 

J.  russ.  phys.  Chem.  Soc. — Journal  de  la  Societe"  physico-chemique  russe.    St.  P£tersbourg. 
J.  Russ.  Soc. — Journal  of  the  Russian  Chemical  Society.    St.  Petersburg,   1869-1315+. 

47  vols. 
J.  Soc.  Chem.  Ind. — Journal  of  the  Society  of  Chemical  Industry.    London,  1882-1915+ . 

34  vols. 

J.  S.  C.  I.— See  above. 

J.  Tok.  Chem.  Soc. — Journal  of  the  Tokyo  Chemical  Society. 
Kastn.  Arch. — Archiv  fur  die  gesammte  Naturlehre,  edited  by  Kastner.    Nuremberg,  1824- 

35.     25  vols. 

Listy  Chemicke*. — Listy  Chemicke",  edited  by  Preis  and  others.    Prague 
Lond.  R.  Soc.  Proc. — See  Roy.  Soc.  Proc. 
Lund.  Univ .  Arsk. — Lunds  Universitets  Ars-skrift.    Lund. 


ABBREVIATIONS  OF  REFERENCES 


xvii 


Dd  VerWandter  Theile  der  anderer  Wissenschaften.    Vienna, 

M'  A'  ABi;"^Sit?llligsb?^chte          mathematisch-physikalischen  Classe  der  kgl.  bayerischen 

Akademie  der  Wissenschaften  zu  Munchen. 
Mag.  Pharm. — Magazin  der  Pharmacie.    1823-31.    36  vols 
Mem.  Acad.  St.  PStersb.— M^moires  de  TAcad^mie  Imp&iale  des  Sciences  de  Saint-Peters- 

M.  Ch.— See  M. 

Mem  CoUSci.  Kyoto.— Memoirs  of  the  College  of  Science,  Kvoto. 

Metall. — Metallurgie.     Halle. 

Miner.  Jahrb. — Neues  Jahrbuch  fnr  Mineralogie,  etc.    1833-73.    40  vols 

Miner.  Mag. — Mineralogical  Magazine.    London. 

Miner.  Mitt— Mineralogische  und  petrographische  Mitteilungen     Wien 

Momt.  Scient.— Le  Moniteur  Scientifique,  edited  by  Quesnesville.     Paris. 

N.  Arch.  Sc.  ph.  nat—  Nouvelles  Archives  des  Sciences  physiques  et  naturelles.    Geneva. 

N.  Cim.— II  nuovo  Cimento.    Pisa,  1855-61.    14  vols 

N.  Edinb.  Phil.  J.— New  Edinburgh  Philosophical  Journal.    1819-64.    90  vols. 

N.  Jahrb.  Miner.— Neues  Jahrbuch  fur  Mineralogie.    Stuttgart. 

N.  Jahrb.  Pharm. — Neues  Jahrbuch  der  Pharmacie.    1796-1840.    42  vols. 

N.  J.  Pharm.— Neues  Journal  der  Pharmacie  fur  Aerzte,  etc.,  edited  by  Trommsdorff. 

1817-34.     27  vols. 

N.  Rep.  Pharm. — Neues  Repertorium  fur  Pharmacie.    1852-76.    25  vols. 
Pharm.    Centralbl.— Pharmaceutisches    Centralblatt.     1830-49.     20  vols.     Continued  as 

O.  O. 

Pharm.  Era. — Pharmaceutical  Era. 

Pharm.  J.  Trans. — Pharmaceutical  Journal  and  Transactions. 
Pharm.  Post. — Pharmaceutische  Post.  Wien. 
Pharm.  Vierteljb.— Pharmaceutische  Vierteljahresberichte. 
Pharm.  Weekbl. — Pharmaceutisches  Weekblad. 
Pharm.  Ztg. — Pharmaceutische  Zeitung. 

Phil.  Mag.— The  Philosophical  Magazine.    London.    1st  series,  1814-26,  26  vols.  ;  2nd  series, 
1827-32,  11  vols.;  3rd  series,  1832-50,   37  vols.;  4th  series,    1851-75,  50  vols.;  5th 
series,  1876-1900,  50  vols.;  6th  series,  1901-1915 +,  30  vols. 
Phil.  Mag.  Ann. — The  Philosophical  Magazine  and  Annals  of  Chemistry,  etc.    Corresponds 

to  Phil.  Mag.  2nd  series. 

Phil.  Trans.— The  Philosophical  Transactions  of  the  Royal  Society  of  London.    1665-1915+ . 
Phys.  Rev. — The  Physical  Eeview. 

Pogg. — Annalen  der  Physik  und  Chemie,  edited  by  Poggendorf .     1st  series,  1824-43,  60  vols. ; 
2nd  series,  1844-53,  30  vols.;  3rd  series,  1854-63,  30  vols.;  4th  series,  1864-73,  30 
vols.;  5th  series,  1874-77,  10  vols.    Continued  as  W.  Ann. 
Polyt.  Centralbl.— Poly technisches  Centralblatt.      1st  series,  1835-46,  12  vols.;  2nd  series, 

1847-73,  30  vols. 
Proc.  Am.  A.  A.  S. — Proceedings  of  the  American  Association  for  the  Advancement  of 

Science. 
Proc.  Am.  Acad. — Proceedings  of  the  American  Academy  of  Arts  and  Sciences.     Boston, 

1846-19 15+.     50  vols. 

Proc.  Am.  Phil.  Soc. — Proceedings  of  the  American  Philosophical  Society.     Philadelphia. 
Proc.  Chem.  Soc. — Proceedings  of  the  Chemical  Society  of  London. 
Proc.  K.  Akad.  Wet.— See  Ver.  K.  Akad.  Wet. 

Proc.  Soc.  Manchester. — Proceedings  of  the  Literary  and  Philosophical  Society  of  Manchester. 
Proc.  Roy.  Soc.— See  Roy.  Soc.  Proc. 

Q.  J.  Sci—  Quarterly  Journal  of  Science.    London,  1816-26.    22  vols. 
Rass.  Min. — Rassegna  mineraria,  metallurgica  e  chirnica. 
Real.  Ac.  Line. — Atti,di  Reale  Accademia  dei  Lincei.    Rome. 
Rend.  Ac.  Line.    See  Att.  Ac.  Line. 

Rep.  anal.  Ch. — Repertorium  der  analytischen  Chemie.    1881-87.    7  vols. 
Rep.  Brit.  Assn.  Adv.  Sci. — Reports  of  the  Meetings  of  the  British  Association  for  the  Ad- 
vancement of  Science. 
Repert. — See  Rep.  Pharm. 

Repert.  chim.  appl. — Repertoire  de  Chimie  pure  et  applique*e.    Paris,  1858-63.    9  vols. 
Rep.  Pharm. — Repertorium  fiir  die  Pharmacie,  edited  by  Buchner.    1st  series,  1815-34,  50 
vols.;  2nd  series,  1835-48,  50  vols.  ;  3rd  series,  1849-51,  10  vols.     Continued  as  N.  Rep. 
Pharm. 

Rev.  ge*n.  chim. — Revue  generate  de  chimie  pure  et  applique"e. 
Rev.  Met. — Revue  de  Metallurgie.    Paris. 
Roy.  Soc.  Proc. — Proceedings  of  the  Royal  Society  of  London.    1832-1915+.    92  vols. 


xviii     .  ABBREVIATIONS  OF  REFERENCES 

Roy.  Soc.  Trans.— Abstracts  of  Philosophical  Transactions  of  the  Royal  Society  of  London. 
1832-54.    6  vols.    Continued  with  Roy.  Soc.  Proc. 

R.  t.  c. — Recueil  des  Travaux  chimiques  des  Pays-Bas.    Leiden,  1882-1915+.    34  vols. 

Russ.  Zeit.  Pharm. — Pharmaceutische  Zeitschrift  fur  Russland. 

Scheik  Verhandel. — Scheikundige  Verhandelingen  en  Onderzoekingen,   edited  by  Mulder. 
Rotterdam,  1857-64.    3  vols. 

Scher.  J.— Allgemeines  Journal  der  Chemie,  edited  by  Scherer.     1798-1810.    17  vols.    Con- 
tinued as  Schw.  J. 

Schw.  J.— Journal  fiir  Chemie  und  Physik,  edited  by  Schweigger.     1st  series,  1811-20,  30 
vols.;  2nd  series,  1821-30,  30  vols.;  3rd  series,  1831-33,  9  vols.    Continued  as  J.  pr. 

Sill.  Am.  J. — American  Journal  of  Science,  edited  by  Silliman,  etc.    See  Am.  J.  Sci. 

Sitzungsb.    bohms.    Gesell. — Sitzungsberichte  der  koniglichen  bohmschen  Gesellschaft  der 
Wissenschaften  in  Prag. 

Storer's  Diet. — First  Outlines  of  a  Dictionary  of  Solubilities  of  Chemical  Substances,  by 
F.  H.  Storer.    Boston,  1864. 

Sv.  V.  A.  F. — Ofversigt  af  kongl.  Svenska  Vetenskaps-Akademien  Forhandlingar.     Stock- 
holm. 

Sv.  V.  A.  H. — Kongliga  Svenska  Vetenskaps-Akademiens  Handlingar.     Stockholm. 

Sv.  V.  A.  H.  Bih. — Bihang  till  kongl.  Svenska  Vetenskaps-Akademiens  Handlingar.    Stock- 
holm. 

Techn.  J.  B. — Jahresbericht  iiber  die  Fortschritte  der  chemischen  Technologie,  edited  by 
Wagner,  Fischer,  etc. 

Trans.  Am.  Electrochem.  Soc. — Transactions  of  the  American  Electrochemical  Society. 
Philadelphia. 

Trans.  Faraday  Soc. — Transactions  of  the  Faraday  Society.    London. 

Trans.  Roy.  Soc. — Philosophical  Transactions  of  the  Royal  Society  of  London. 

Ver.  K.  Akad.  Wet. — Verslag  Koninkle  Akademie  van  Wettenschappen,  Amsterdam. 

W.  A.  B. — Sitzungsberichte  der  mathematisch-naturwissenschaftlichen  Classe  der  kaiser- 
lichen  Akademie  der  Wissenschaften  zu  Wien. 

W.  Ann. — Annalen  der  Physik  und  Chemie,  edited  by  Wiedemann.    Continuation  of  Pogg 
1877-1899.    69  vols.    4th  series,  1900-1915 +.    48  vols. 

W.  Ann.  Beibl. — Beiblatter  zu  Wiedemann's  Annalen.    Leipzig. 

Z.  anal. — Zeitschrift  fiir  analytische  Chemie,  edited  by  Fresenius.    Wiesbaden,  1862-1915  +  . 
54  vols. 

Z.  anorg. — Zeitschrift  fiir  anorganische  Chemie,  edited  by  Krtiss.    1892-1915+.    93  vols. 

Z.  B.  H.  Sal. — Zeitschrift  fur  das  Berg,  Hiitten,  und  Salinen-Wesen  in  dem  preussischen 
Staate.     Berlin. 

Zeit.  angew.  Ch.— Zeitschrift  fur  angewandte  Chemie.    Berlin,  1887-19 15+.    29  vols. 

Zeit.  Chem. — Zeitschrift  fiir  Chemie  und  Pharmacie.     1st  series,  1858-64,  6  vols.'  2nd  series 
"N.  F.,"  1865-71,  7  vols. 

Zeit.  d.  allgem.  oster.    Apothekerv. — Zeitschrift  des  allgemeinen  osterreichischen  Apotheker- 
vereins. 

Zeit.  ges.  Nat. — Zeitschrift  fiir  die  gesammten  Naturwissenschaften. 

Zeit.  Krist. — Zeitschrift  fiir  Krystallographie  und  Mineralogie.    1877-1915+ .    51  vols. 

Zeit.  Pharm. — See  Russ.  Zeit.    Pharm. 

Z.  Elektrochem. — Zeitschrift  fiir  Elektrochemie.    Halle. 

Z.  Phys.  Ch. — Zeitschrift  fiir  physikalische  Chemie,  edited  by  Oswald  and  van't  Hoff     1887- 
1915+.     90  vols. 

Z.  physiol.  Chem. — Zeitschrift  fiir  physiologische  Chemie.    Strassburg. 

Z.  Ver.  Zuckerind. — Zeitschrift  des  Verein  der  deutschen  Zuckerindustrie. 


A  DICTIONARY  OF  CHEMICAL  SOLUBILITIES 


INORGANIC 


DICTIONARY 


OP 


CHEMICAL   SOLUBILITIES 

INORGANIC 


Actinium  emanation. 

Solubility  coefficient  of  actinium  emanation 
in  H2O  at  room  temp,  is  2. 

If  the  solubility  of  actinium  emanation  in 
H2O  is  made  =  1,  the  relative  solubility  of  the 
emanation  in  sat.  KCl+Aq  =  0.9;  in  cone. 
H2SO4  =  0.95;  in  ethyl  alcohol  =  1.1;  in  amyl 
alcohol  =  1.6;  in  benzaldehyde  =  1.7;  in  ben- 
zene =  1.8;  in  toluene  =  1.8;  in  petroleum  = 
1.9;  inCS2  =  2.1  at  18°. 

(Hevesy,  Phys.  Zeit.  1911, 12. 1221.) 


Air,  Atmospheric. 

See  also  Nitrogen  and  Oxygen. 

100  vols.  H2O  at  15°  and  760  mm.  absorb  about  5 
vols.  atmospheric  air.     (Saussure.) 

1  vol.  H2O  at  t°  and  760  mm.  pressure  absorbs 
V  vols.  atmospheric  air  reduced  to  760  mm. 
and  0°. 


0.02471 
0.02406 
0.02345 
0.02287 
0.02237 
0.02179 
0.02128 


9 
10 
11 
12 
13 


0.02080 
0.02034 
0.01192 
0.01953 
0.01916 
0.01882 
0.01851 


14 
15 
16 
17 

18 
19 
20 


0.01822 
0.01795 
0.01771 
0.01750 
0.01732 
0.01717 
0.01701 


(Bunsen's  Gasometry.) 


1 1.  H2O  absorbs  cc.  N  and  O  from  air  at  tc 
and  760  mm.  pressure. 


cc. 

cc. 

t° 

N 

O 

N+O 

0 

16.09 

8.62 

24.71 

5 

14.18 

7.60 

21.78 

10 

12.70 

6.79 

19.49 

15 

11.67 

6.25 

17.92 

20 

11.08 

5.93 

17.01 

(Bunsen,  Gasometr.  Methoden,  2te  Aufl.  209, 
220.) 


1 1.  H2O  absorbs  cc.  N  and  O  from  air  at  t° 
and  760  mm.  pressure  (dry). 


t° 

cc.  N 

cc.   O 

N+O 

%o 

10 

15.47 

7.87 

23.34 

33.74 

15 

13.83 

7.09 

20.92 

33.86 

20 

12.76 

6.44 

19.20 

'  33.55 

25 

11.78 

5.91 

17.69 

33.40 

(Roscoe  and  Lunt,  Chem.  Soc  55.  568.) 

1 1.  H2O  absorbs  cc.  N  and  O  from  air  at  t° 
and  760  mm. 


0 

6.0 

6.32 

9.18 

13.70 

14.10 


cc.  N 


19.53 
16.34 
16.60 
15.58 
14.16 
14.16 


cc.  O 


10.01 
8.28 
8.39 
7.90 
7.14 
7.05 


%o 


33.88 
33.60 
33.35 
33.60 
33.51 
33.24 


(Pettersson  and  Sonde"n,  B.  22.  1439.) 

1  1.  H2O  absorbs  cc.  N  (0°  and  760  mm.) 
from  atmospheric  air  at  t°  and  760  mm. 
pressure  (dry). 


cc.  N 


19.14 
18.20 
17.34 
16.54 
15.81 


10 
12 
14 
16 

18 


cc.  N 


15.14 
14.53 
13.98 
13.48 
13.03 


20 
22 
24 
25 


cc.  N 


12.63 
12.27 
11.95 
11.81 


(Hamberg,  J.  pr.  (2)  33.  447.) 

1  1.  H2O  absorbs  cc.  N  from  air  at  t°  and 
760  mm.  pressure. 


cc.  N 


19.29 
17.09 


t° 


10 
15 


cc.  N 


15.36 
13.95 


20 
25 


cc.  N 


12.80 
11.81 


(Dittmar,  Challenger  Expedition,  vol.  1.  pt.  1.) 


AIR,  ATMOSPHERIC 


1  1.  H20  sat.  with  air  at  tc  and  760  mm.  con- 

j.     •           -_      f\    f       j  '    j.  _    "no    _2iJ  ,«*/a/\'  ^.'  V 

.*  .    Solubility  of  atmos.  etc.  —  Continued 

tains  cc.  \J  (.rec1 

.to  y,   auu  fou  imn.^.  .;t 

^T'&mn 

Nitrogen 

Temp 

Oxygen 

Nitrogen. 

t°         cc.  O 

t° 

cc.  O 

t° 

cc.  O 

±  emp 

Uxygen 

(*(* 

PP 

CC. 

CC. 

0     10.187 

11 

7.692 

22 

6.114 

58° 

IfV* 

3.39 

\j\j» 

6.71 

80° 

1.97 

4.03 

1       9.910 

12 

7.518 

23 

5.999 

59 

3.34 

6.60 

81 

1.89 

3.88 

2       9.643 

13 

7.352 

24 

5.886 

60 

3.28 

6.50 

82 

1.81 

3.73 

3       9.387 

14 

7.192 

25 

5.776 

61 

3.22 

6.39 

83 

1.73 

3.57 

4       9.142 

15 

7.038 

26 

5.669 

62 

3.16 

6.27 

84 

1.65 

3.41 

5       8.907 

16 

6.891 

27 

5.564 

63 

3.10 

6.16 

85 

1.57 

3.24 

6       8.682 

17 

6.730 

28 

5.460 

64 

3.04 

6.05 

86 

1.48 

3.07 

7       8.467 

18 

6.614 

29 

5.357 

65 

2.98 

5.94 

87 

1.39 

2.89 

8       8.260 

19 

6.482 

30 

5.255 

66 

2.92 

5.82 

88 

1.30 

2.71 

9       8.063 

20 

6.356 

.  . 

67 

2.85 

5.70 

89 

1.21 

2.52 

10       7.873 

21 

6.233 

... 

68 

2.79 

5.59 

90 

1.11 

2.32 

(Winkler,  B.  22.  1773.) 

69 
70 

2.73 
2.66 

5.47 
5.35 

91 
92 

1.02 
0.92 

2.12 
1.91 

1  vol.  H20  absorbs  0.01748  vol.  air  at  24.05° 
•and  760  mm.  pressure.      (Winkler,   B.   21. 

71 
72 
73 

2.60 
2.53 
2.47 

5.23 
5.10 
4.98 

93 
94 
95 

0.81 
0.71 
0.60 

1.70 
1.48 
1.25 

Composition  of  the  absorbed  air  between  0° 
and  24°  is  34.91%  O  and  65.09%  N  (Bunsen)  ; 
between  15°  and  16°,  32.17%  O  and  67.83%  N 
(Konig  and  Kranch,  Z.  anal.  19.  259);  32% 
0  and  68%  N  (Regnault);  at  0°,  35.1%  O; 
10°,  34.8%  0;  20°,  34.3%  0;  25°,  33.7%  O 
(Winkler,  B.  21.  2483).    See  also  Roscoe  and 

74 
75 
76 

77 
78 
79 

2.40 
2.33 
2.26 
2.19 
2.12 
2.04 

4.85 
4.72 
4.59 
4.45 
4.32 
4.18 

96 
97 
98 
99 
100 

0.48 
0.37 
0.27 
0.13 
0.00 

1.01 
0.77 
0.52 
0.27 
0.00 

(Winkler,  B.  1901,  34.  1440.) 

Lunt,  and  Pettersson  and  Sonden,  page  1. 

Absorption  of  atmospheric  air  by 

H2O  at  t° 

Solubility  of  atmos.  oxygen  and  nitrogen 
in  1000  cc.  H2O  at  760  mm.  pressure  (calc.). 

and  760  mm.  pressure.     £  =  coefficient  of 
absorption.        £1  =  "  Solubility."       (See 
under  oxygen.) 

Temp 

Oxygen 

Nitrogen 

Temp 

Oxygen 

Nitrogen 

t° 

ft 

0i 

t° 

0 

/3i 

0° 

1 

2 
3 
4 
5 
6 
7 
8 
9 

CC. 
10.19 

9.91 
9.64 
9.39 
9.14 
8.91 
8.68 
8.47 
8.26 
8.06 

CC. 

18.45 
17.99 
17.55 
17.12 
16.71 
16.30 
15.91 
15.54 
15.18 
14.83 

29° 
30 
31 
32 
33 
34 
35 
36 
37 
38 

CC. 

5.33 
5.24 
5.15 
5.07 
4.99 
4.91 
4.83 
4.76 
4.69 
4.62 

CC. 

10.30 
10.15 
9.99 
9.83 
9.67 
9.52 
9.37 
9.22 
9.08 
8.94 

0 
5 
10 
15 
20 
25 
30 
35 
40 
45 

KA 

3.02881 
2543 
2264 
2045 
1869 
1724 
1606 
1503 
1418 
1351 

19Q7 

3.02864 
2521 
2237 
2011 
1826 
1671 
1539 
1420 
1315 
1224 
1  1  d.n 

55 

60 
65 
70 
75 

80 
85 
90 
95 
100 

0.01253 
1216 
1182 
1156 
1137 
1126 
1119 
1113 
1109 
1105 

0.01059 
0978 
0892 
0801 
0705 
0600 
0481 
0343 
0185 
0000 

10 

7.87 

14.50 

39 

4.55 

8.81 

ou 

l.A\J  1 

114:U 

11 

7.69 

14.19 

40 

4.48 

8.67 

(Winkler,  B.  1901,  34.  1409.) 

12 

7.52 

13.8k 

} 

41 

4.42 

8.55 

13 

7  35 

1361 

42 

4.35 

8.43 

Sea-water  absorbs  less  O  and  N  from  air 

14 

i.  19 

13.33 

43 

4.28 

8.31 

than  pure  H2O,  but  the  ratio  between  O  and  N 

15 

7.04 

13.07 

44 

4.22 

8.20 

remains  constant.    In  sea-water  sat.  with  air 

16 

6.89 

12.83 

45 

4.15 

8.09 

at  6.22°  the  oxygen  was  33.50%  of  the  total 

17 

6.75 

12.57 

46 

4.09 

7.97 

gas  absorbed.    (Pettersson  and  Sonde"n.) 

18 

6.61 

12.34 

47 

4.03 

7.87 

1  1.  sea-water  absorbs  cc.  N  and  O  from  air 

19 

6.48 

12.12 

48 

3.97 

7.76 

at  t°  and  760  mm.  pressure. 

20 

6.35 

11.91 

49 

3.91 

7.65 

21 

6.23 

11.71 

50 

3.85 

7.55 

t° 

cc.  N 

CC.  O 

N+0 

%  o 

00 

fi  in 

UX.r 

> 

51 

3.79 

7  4V 

mm 

23 

U»  \\j 

5.98 

*<J4j 

11.33 

tPJL 

52 

3J4 

*  »^«J 

7.34 

0 

14.41 

7.77 

22.18 

35.03 

24 

5.86 

11.14 

53 

3.68 

7.24 

5 

13.22 

6.93 

20.15 

34.39 

25 

5.75 

10.96 

54 

3.62 

7.13 

10 

12.08 

6.29 

18.37 

34.24 

26 

5.64 

10.79 

55 

3.56 

7.03 

15 

11.01 

5.70 

16.71 

34.11 

27 
28 

5.54 
5.43 

10.62 
10.46 

56 
57 

3.51 
3.45 

6.92 
6.81 

Cl'ornoe,  ^Norwegian  JNorth  Atlantic  Exped. 
Chem.  18.) 

ALUMINATE,  CALCIUM 


1  1.  sea  water  absorbs  cc.  X  from  air  at  t° 
and  760  mm. 

Alum,  Ammonia, 
See  Sulphate,  aluminum  ammonium. 
Alum,  Chrome. 
See  Sulphate,  aluminum  chromium. 
Alum,  Iron, 
See  Sulphate,  aluminum  ferric. 
Alum,  Potash. 
See  Sulphate,  aluminum  potassium. 
Alumina. 
See  Aluminum  oxide. 

Aluminic  acid,  H2A12O4  =  A12O3,  H2O. 
Aluminum  hydroxide  possesses  acid  prop- 
erties, and  salts  corresponding  to  an  acid  of 
the  above  formula  exist. 
See  Aluminum  hydroxide. 

t° 

0 
5 

cc.  N 

15.60 
13.86 

t° 

cc.  X 

t 

20 
25 

cc.  N 

10.41 
9.62 

10 
15 

12.47 
11.34 

(Dittmar.) 

1  1.  sea-water  absorbs  cc.  N  (0°  and  760  mm.) 
from  atmospheric  air  at  t°  and  760  mm. 
pressure  (dry). 

t° 

cc.  N 

14.85 
14.20 
13.60 
13.04 
12.53 

t° 

cc.  N 

t° 

cc.  N 

10.25 
9.98 
9.73 
9.62 

0 
2 

4 
6 

8 

10 
12 
14 
16 

18 

12.06 
11.62 
11.23 
10.87 
10.54 

20 
22 
24 
25 

Absorption  of  air  which  is  free  from  car- 
bonic acid  by  H2SOf  at  18°  and  760  mm.  a  = 
coefficient  of  solubility. 


H2SO4 

a 

H2SO4 

a 

98% 
90% 
80% 

0.0173 
0.0107 
0.0069 

70% 
60% 
50% 

0.0055 
0.0059 
0.0076 

(Tower,  Z.  anorg.  1906,  50,  388.) 

Absolute  alcohol  absorbs  0.11  vol.  gas  from  air,  l/a  of 

which  is  O  and  2/s,  N.     On  mixing  with  an  equal  vol. 

HaO,  2/»  of  the  dissolved  gas  is  given  off.     (Dobereiner.) 

100  vols.   alcohol   (95.1  %)    absorb    14.1   vols.   air. 

(Robinet,  C.  R.  58.  608.) 

100  vols.  petroleum       absorb  6.8    vols.  air. 

"     oil  of  lavender   "        6.89     ' 
"       "     benzene  14.0 

"       "     oil  of  turpentine"     24.18     ' 
(Robinet,  I.e.) 

1  vol.  ether  at  760  mm.  pressure  absorbs 
0.290  vols.  air  at  0°;  0.287  vols.  at  10°; 
0.286  vols.  at  15°.  (Christoff,  Z.  phys.  Ch. 
1912,  79.  459.) 

Alcohol.    C2H5OH. 

Sp.  gr.  of  pure  ethyl  alcohol +Aq.  at  25°. 


alcohol 

Sp.  gr. 

% 

alcohol 

Sp.  gr. 

0 

0.997077 

55 

0.898502 

2 

0.993359 

60 

0.886990 

5 

0.988166 

65 

0.875269 

6 

0.986563 

70 

0.863399 

10 

0.980434 

75 

0.851336 

15 

0.973345 

80 

0.839114 

20 

0.966392 

85 

0.826596 

25 

0.958946 

90 

0.813622 

30 

0.950672 

95 

0.799912 

35 

0.941459 

98 

0.791170 

40 

0.931483 

99 

0.788135 

45 

0.920850 

100 

0.785058 

50 

0.909852 

— 

— 

(Osborne,  McKelvy  and  Bearce,  Bureau  of 
Standards,  Sci.  Paper  No.  197.) 

Aluminates. 

All  aluminates  are  insol.  in  H2O  except 
those  of  K  and  Na  (Fremy)  and  Ba  (Beck- 
mann,  J.  pr.  (2)  26.  385). 

Barium  aluminate,  BaAl2O4+4H2O. 

Sol.  in  10  pts.  H2O;  can  be  recryst.  from 
alcohol.  (Deville,  J.  pr.  87.  299.) 

+5H2O.  SI.  sol.  in  H2O  with  decomp. 
(Allen,  Am.  Ch.  J.  1900,  24.  313.) 

H-7H20.  SI.  sol.  in  cold,  not  completely 
sol.  in  hot  H2O.  Sol.  in  cold  dil.  HCl+Aq. 
(Beckmann,  J.  pr.  (2)  26.  385.) 

Ba2Al205+5H2O.  Sol.  in  20  pts.  H2O  by 
boiling.  (Beckmann,  B.  14.  2151.) 

Insol.  in  alcohol. 

SI.  sol.  in  H2O  with  decomp.;  insol.  in 
alcohol.  (Allen,  Am.  Ch.  J.  1900,  24.  311.) 

Ba3Al2O6+7~llH2O.  Sol.  in  15  pts.  H20 
with  decomp.  into  Ba2Al2Os+5H2O;  insol.  in 
alcohol.  (Beckmann.) 

Barium  aluminate  bromide,  BaAl2O4,  BaBr2 

+  11H2O. 
Sol.  in  H2O.    (Beckmann,  J.  pr.  (2)  26.  385, 

474.) 

Barium  aluminate  chloride,  BaAl2O4,  3BaCl2 
+6H2O. 

Sol.  in  H2O.    (Beckmann,  I.e.) 

BaAl2O4,  BaCl2+llH2O.  Sol.  in  H2O. 
(Beckmann,  I.e.) 

Barium  aluminate  iodide,  BaAl2O4,  BaI2. 
Sol.  in  H2O.    (Beckmann,  I.e.) 

Calcium  aluminate,  CaO,  A12O3, 

Decomp.  by  H2O  but  does  not  "set."  Sol. 
in  HC1;  insol.  in  HNO3,  H2SO4,  and  HF. 
(Dufau,  C.  R.  1900,  131.  543.) 

Ca2Al2O6-f7H2O.  Slowly  decomp,  by 
H2O;  si.  sol.  in  H2O.  (Allen,  Am.  Ch.  J. 
1900,  24.  316.) 

Ca3Al2Oe.  Insol.  in  H2O;  not  decomp.  by 
KOH+Aq;  sol.  in  acids.  (Tissier,  C.  R.  48. 
627.) 


ALUMINATE,  COBALT 


+6H2O.  Ppt;  si.  sol.  in  H2O;  insol.  i 
alcohol.  (Allen,  Am.  Ch.  J.  1900,  24.  316.) 

3Al2O3.4CaO+3H2O.  Ppt.  (Friedel,  Bui 
Soc.  Min.  1903,  26.  121;  C.  C.  1904,  I.  430. 

Cobalt  aluminate. 

"Thenard's  or  Leithner's  blue."  Insol.  i 
H20. 

CoAl2O4.  Insol.  in  H2O  and  acids.  (Ebel 
men.) 

Cobalt  magnesium  aluminate,  [MgCo]Al2O4 

"Spinel  Blue.1'    Insol.  in  H2O  or  HCl+Aq 

(Ebehnen.) 

Glucinum  aluminate,  G1A12O4. 

Min.  Chrysoberyll.  Not  attacked  by  acids 
but  decomp.  by  KOH+Aq. 

Iron  (ferrous)  aluminate,  FeAl2O4. 

Min.  Hercynite.    Not  attacked  by  acids. 
Lithium  aluminate,  LiAlO2. 

Sol.  in  H2O.  (Weyberg,  C.  C.  1906,  II 
1659.) 

Lithium    hydrogen    aluminate,    LiHAl2O4  + 

5H20. 

SI.  sol.  in  H2O;  decomp.  on  boiling.  (Allen 
Am.  Ch.  J.  1900,24.310.) 

Magnesium  aluminate,  MgAl2O4. 

Min.  Spinel.    Insol.  in  H2O. 

Insol.  in  HNO3+Aq;  very  si.  sol.  in  HC1 
-f  Aq;  partly  sol.  in  H2SO4  at  boiling  temp. 
(Abich,  Pogg.  23.  316.) 

Sol.  by  standing  2  hours  at  210°  with  a 
mixture  of  3  pts.  H2SO4  and  1  pt.  H20,  or  by 
boiling  with  this  mixture  together  with  HF. 
(Mitscherlich,  J.  pr.  81.  108.) 

SI.  sol.  in  HC1,  HF,  and  H2SO4;  insol.  in 
HNO3.  (Dufau,  Bull.  Soc.  1901,  (3)  26. 669.) 

Manganous  aluminate. 

Insol.  in  H2O  and  acids.  (Ebelmen,  A.  ch. 
(3)  22.  225.) 

MnAl2O4.  Insol.  in  HCl+Aq;  readily 
attacked  by  HF,  HNO3  and  H2SO4. 

Decomp.  by  fusion  with  alkali  chlorate, 
nitrate,  oxide  or  carbonate.  (Dufau,  C  R 
1902,  136.  963.) 

Nickel  aluminate. 

Insol.  in  H2O. 
Potasssium  aluminate,  K2A12O4+3H2O. 

Decomp.  by  dissolving  in  pure  H2O  with 
separation  of  A12O3.  (Fremy,  A.  ch.  (3).  12. 
362.)  Can  be  recrystallised  from  water  con- 
taining a  little  alkali,  without  decomposition. 
(Fremy.) 

Insol.  in  alcohol. 

Sodium  aluminate,  Na2Al2O4. 

Easily  and  completely  sol.  in  cold  H2O. 
(Schaffgotsch,  Pogg.  43.  117.) 

+4H2O.  Insol.  in  alcohol.  (Allen,  Am. 
Ch.  J.  1900,  24.  308.) 


e.  Miscible  with  hot  H2O,  and  as 
sol.  as  NaOH  in  cold  H2O.  Insol.  in  alcohol 
but  decomp.  thereby.  (Tissier,  C.  R.  43.  102.) 

Strontium  aluminate,  Sr3Al2O6+6H20. 

SI.  sol.  in  H2O  (with  slow  decomp.  in  Aq. 
solution).    (Allen,  Am.  Ch.  J.  1900,  24.  314.) 


Thallium  aluminate, 

Not  completely  sol.  in,  but  slowly  hydro- 
lysedbyH2O. 

Readily  sol.  in  dil.  acids  and  in  the  fixed 
alkalies. 

Insol.  in  abs.  alcohol.  (Hawley,  J.  Am. 
Chem.  Soc.  1907,  29.  303.) 

Zinc  aluminate,  ZnAl204. 

Insol.  in  acids  or  alkalies. 

Min.  Gahnite  (Automolite). 

+zH20.  Sol.  in  KOH,  and  NH4OH+Aq. 
(Berzelius.) 

Aluminicoantimoniotungstic  acid. 

Ammonium        aluminicoantimoniotungstate, 

6(NH4)20,    2A1203,    3Sb205,     18WO3  + 
17H2O. 

A  shellac-like  gum.  (Daniels,  J.  Am.  Chem. 
Soc.  1908,  30.  1856.) 

Barium  aluminicoantimoniotungstate,  5BaO, 

2A12O3,  3Sb2O6,  18W03+6H2O. 
Somewhat  insol.   in  dil.   HC1.     (Daniels, 
J.  Am.  Chem.  Soc.  1908,  30.  1857.) 

Silver  aluminicoantimoniotungstate,  6Ag2O, 

2A1203,  3Sb2O5,  18WO3+12H2O. 
Ppt. 

Sol.  in  NH4OH+Aq  but  requires  HNO3 
1:10)  to  dissolve  it.    (Daniels,  J.  Am.  Chem. 
Soc.  1908,  30.  1857.) 

Aluminicoarseniotungstic  acid. 

Ammonium  aluminicoarseniotungstate. 
6(NH4)20,  2A1203,  3As205,  18W08  + 
14H2O. 

Sparingly  sol.  in  H2O.  (Daniels,  J.  Am. 
!hem.  Soc.  1908,  30.  1854.) 

Barium  aluminicoarseniotungstate,  4BaO, 
2A12O3,  3As206,  18WO3  +  12H2O. 

Very  si.  sol.  in  H2O. 

Sol.  in  very  dil.  HC1  or  HN03.  (Daniels, 
T.  Am.  Chem.  Soc.  1908,  30.  1855.) 

Cadmium  aluminicoarseniotungstate.  4CdO 

2A12O3,  3As2O6,  18WO3+17H2O. 
Sol.  in  dil.  mineral  acids  and  in  strong 


Aluminicomolybdic  acid. 

Ammonium  aluminicomolybdate,  3(NH/)9O 

A12O3,  12MoO3+19H2O. 
Ppt.    (Hall,  J.  Am.  Chem.  Soc.  1907,  29. 

+20H2O.    More  sol.  in  H20  than  potassium 


ALUMINUM 


aluminicomolybdate.    (Struve,  Bull.  Acad.St. 
Petersb.  12.  147.) 

+22H2O.    (Marckwald,  Dissert.  1895.) 

Barium   aluminicomolybdate,   4BaO,   A12O3, 

12MoO3+14H2O. 

Ppt.  (Hall,  J.  Am.  Chem.  Soc.  1907,  29. 
712.) 

Lead     aluminicomolybdate,     4PbO,     A12O3, 

12MoO3+21H2O. 
Ppt.     (Hall,  J.  Am.  Chem.  Soc.  1907,  29. 

712.) 

Potassium  aluminicomolybdate,  3K2O,  A12O3, 
12Mo03+20H2O. 

1  pt.  of  the  salt  is  sol.  in  40.67  pts.  H2O  at 
17°.  Very  difficultly  sol.  in  acids.  (Struve.) 

H3Al(MoO4)3,  2KHMoO4.  Sol.  in  H2O. 
(Parmentier,  C.  R.  94.  1713.) 

Silver    aluminicomolybdate,    4Ag2O,    A12O3, 

12MoO3+16H2O. 

Ppt.  (Hall,  J.  Am.  Chem.  Soc.  1907,  29. 
712.) 

Sodium   aluminicomolybdate,  3Na2O,  A12O3, 

12Mo03+22H2O. 

Efflorescent.  Easilv  sol.  in  HoO.  (Gentele 
J.  pr.  81.  413.) 

Aluminicophosphotungstic  acid. 

Ammonium  aluminicophosphotungstate, 

9(NH4)20, 2A12O3, 4P2O5, 9WO3  +  13H2O. 
SI.  sol.  in  cold  and  in  hot  H2O.     (Daniels, 
J.  Am.  Chem.  Soc.  1908,  30,  1851.) 

Barium    aluminicophosphotungstate,    4BaO, 

2A12O3,  4P2O5,  9WO3  +  13H2O. 
SI.  sol.  in  HoO.     Sol.  in  very  dil.  HC1  or 
HNO3.     (Daniels,  J.  Am.  Chem.  Soc.  1908, 
30.  1853.) 

Silver     aluminicophosphotungstate,     4Ag2O, 

'  2A120S,  4P2O6,  9WO3+6H2O. 

Nearly  insol.  in  H2O.  Sol.  in  NH4OH  and 
in  dil.  HN03.  Insol.  in  acetic  acid.  (Daniels, 
J.  Am.  Chem.  Soc.  1908,  30.  1852.) 

Zinc       aluminicophosphotungstate,       5ZnO, 

2A12O3,  4P?O6,  9WO3  +  11H2O. 
Sol.  in  dil.  acids  and  in  a  large  quantity  of 
cone,    ammonia    when    NH4C1    is    present. 
(Daniels,    J.    Am.    Chem.    Soc.    1908,    30. 
1853.) 

Aluminicotungstic  acid. 

Ammonium    aluminicotungstate,    3(NH4)2O, 

A12O3,  9WO3+4H2O. 

Sol.  in  cone.  HNO3  and  in  cone.  HC1.  When 
the  solution  in  cone.  HC1  was  boiled,  a  yellow 
colored  ppt.  separated.  (E.  F.  Smith,  J.  Am. 
Chem.  Soc.  1903,  25.  1230.) 

Ammonium      silver       alumininicotungstate, 

HAg2O,  21(NH4)2O,  4A12O3;  36WO3. 
The  dry  salt  is  insol.  in  pure  H2O,  but 


readily  sol.  in  H20  containing  NH3  or  HNO3. 
(E.  F.  Smith,  J.  Am.  Chem.  Soc  1903.  25. 
1231.) 

Barium    aluminicotungstate,    SBaO.    A1<>O3. 

9W03+7H20. 

Not  sol.  in  acids  when  dry.  Somewhat 
decomp.  by  boiling  with  cone.  HC1,  HNO3  or 
aqua  regia.  (Daniels,  J.  Am.  Chem.  Soc. 
1908,  30.  1848.) 

Copper    aluminicotungstate,    2CuO,    A1203, 


Sol.  in  large  quantities  of  H2O.  (Daniels, 
J.  Am.  Chem.  Soc.  1908,  30.  1847.) 

Meicurous  aluminicotungstate,  5Hg2O,  A12O3, 

9WO3. 

SI.  sol.  in  H2O.  Sol.  in  HNO3(1:5).  (Dan- 
iels, J.  Am.  Chem.  Soc.  1908,  30.  1849.) 

Zinc  aluminicotungstate,  IJ^ZnO,  A12O3, 
9WO3+8H2O. 

Insol.  in  H2O.  (Daniels,  J.  Am.  Chem. 
Soc.  1908,  30.  1850.) 

Znp,  A1203,  9WO3+20H2O.  Sol.  in  H2O. 
(Daniels.) 

Aluminum,  Al. 

Less  easily  attacked  than  ordinary  metals 
(iron,  copper,  lead,  zinc,  tin)  by  air,  H2O, 
wine,  beer,  coffee,  milk,  oil,  butter,  fats,  etc. 
Vinegar  dissolves  0.349  g.  from  a  sq.  decimetre 
in  4  months,  and  5  %  NaCl+Aq,  only  0.045 
g.  in  the  same  time.  (Ballaud,  C.  R.  114. 
1536.) 

The  action  of  various  substances  contained 
in  foods  and  drinks  on  compact  Al  as  it  occurs 
in  utensils  is  very  slight.  Hard  or  soft  water, 
whether  cold  or  hot,  showed  no  action  in  8 
days;  1  %  solutions  of  tartaric,  tannic,  and 
acetic  acids  had  no  action  in  same  time,  also 
5  %  boric,  carbolic,  and  salicylic  acids.  4  % 
and  10  %  acetic  acid  dissolved  only  0.4  mg. 
of  Al,  while  10  %  acetic  acid  dissolved  2.1 
mg.  from  a  roughened  piece  of  Al  foil  in  8  days. 
1  %  soda  solution  dissolved  15  mg.  in  8  days. 
(Rupp,  Dingl.  283.  119.) 

Similar  results  were  obtained  by  Arche. 
(Dingl.  284.  255.) 

Liquids  which  are  ordinarily  contained  in 
f  GOG'S  and  drinks  do  not  attack  sheet  Al  ex- 
cept in  a  very  small  degree.  The  following 
losses  in  weight  in  mg.  by  the  action  of  the 
given  liquids  on  100  sq.  centimetres  sheet 
aluminum  for  6  days  were  obtained  : 


Liquids 

Loss  in  mg. 

Claret 
Hock  
Brandy         .          • 
5  %  alcohol 
5  %  tartaric  acid+Aq   . 

1% 
5  %  acetic  acid-|-Aq 

1  07           "        " 

l/c                                     • 

2.84 
3.27 
1.08 
0.61 
1.69 
2.58 
3.58 
4.38 

ALUMINUM, 


Liquids 

Loss  in  mg. 

5  %  citric  acid+Aq 

2.15 

1  %                                   - 

1.90 

5  %  lactic  acid+Aq 

4.77 

5  %  butyric  acid+Aq    . 
Coffee    ' 

1.31 
0.50 

Tea      . 

0 

Beer    

0 

4  %  boric  acid+Aq        .          .  ' 

1.77 

5  %  carbolic  acid+Aq  . 

0.23 

1  %                                   - 

0.49 

^/i  %  salicylic  acid  +  Aq       ,  .  (  f  . 

6.35 

(Lunge,  C.N.  65.  110.) 

The  apparent  solubility  of  this  metal  in 
H2O  is  due  to  the  presence  of  minute  quan- 
tities of  Is1  a.  Absolutely  pure  Al  does  not 
lose  any  weight  to  H2O  and  the  H2O  remains 
perfectly  clear.  Also  dil.  acids  remain  per- 
fectly clear.  (Moissan,  C.  R.  1895,  121. 
794-98;  C.  C.  1896, 1.  193.) 

SI.  attacked  by  H2O  at  80°.  (W.  Smith, 
J.  Soc.  Chem.  Ind.  1904,  23.  475.) 

Easily  sol.  in  dil.  or  cone.  HCl+Aq, 
whether  hot  or  cold;  also  in  HBr.  HI,  or  HF+ 
Aq.  Insol.  in  dil.  H2S04 + Aq  (de  la  Rive) ;  si. 
attacked  by  cold,  easily  by  hot  cone.  H2SO4. 
Not  attacked  by  HNO3+Aq  even  when  cone, 
and  boiling  (Wohler);  easily  sol.  in  dil.  H2SO4, 
or  HNO3+Aq  in  vacuo  (Weeren,  B.  24. 1798) ; 
slowly  sol.  in  27  %  HNO3+Aq,  100  com. 
HNO3+Aq  requiring  2  months  to  dissolve  2 
g.  Al  (Montemartini,  Gazz.  ch.  it.  22.  397); 
very  si.  sol.  in  most  organic  acids,  but  solubil- 
ity is  increased  by  presence  of  NaCl. 

Not  attacked  by  dil.  or  cone.  HNO3  at  ord. 
temp,  but  attacked  by  hot  HNO3.  Attacked 
by  H3PO4.  (Smith,  J.  Soc.  Chem.  Ind.  1904, 
23.  475.) 

Completely  sol.  at  100°  in  two  hours  in 
HNO3,  sp.  gr.  1.15-1.46.  (Stillman,  J.  Am 
Chem.  Soc.  1897,  19.  714.) 

Very  easily  sol.  in  HNO3  (contrary  to  the 
usual  statement  in  text-books).  (Woy,  C.  C 
190  ,  Jl.94.) 

Slowly  attacked  by  HNO3+Aq  (20-25  %) 
at  25-30°.  (Deventer,  Chem.  Weekbl.  1907, 
4.  69.) 

Dil.  HNO3  or  H2SO4  does  not  attack  Al 
on  account  of  formation  of  layer  of  gas.  Ac- 
tion is  increased  by  vacuum.  Solutions  of 
metallic  chlorides,  the  metal  of  which  is  insol. 
and  attaches  itself  to  the  Al  (Pt,  Au,  Cu,  Hg) 
increase  the  solubility,  but  when  metal  is 
soluble  in  the  acid  (Fe,  Zn,  etc.),  there  is  no 
increase  of  solubility.  (Ditte,  C.  R.  1890, 
110.  573.) 

Violently  attacked  by  dil.  or  cone.  H3PO4+ 
Aq.  (Winteler.) 

Not  attacked  by  solution  of  HC1  in  liquid 
HCN.  (Kahlenberg,  J.  phvs.  Chem.  1902, 
6.  662.) 

Very  easily  sol.  in  cone,  or  dil.  KOH,  or 
NaOH+Aq.  Slowly  attacked  by  NH4OH  + 


(Wohler);  sol.  in  BaO2H2+Aq  (Beck- 
mann,  J.  pr.  (2)  26.  385) ;  slowly  sol.  in  CaO2H2 
+Aq. 

Sol.  in  excess  of  10  %  KOH+Aq  and  in 
NaOH  and  LiOH+Aq;  sol.  in  hot  cone. 
Ba(OH)2,  Sr(OH)2  and  Ca(OH)2+Aq.  (Allen, 
Am.  Ch.  J.  1900,  24.  304-331.) 

Attacked  by  hot  cone.  NH4OH+Aq. 
(Smith,  J.  SocfChem.  Ind.  1904,  23.  475.) 

SI.  attacked  by  sulphates,  or  nitrates +Aq, 
but  all  chlorides,  bromides,  and  iodides,  except 
those  of  the  alkalies  and  alkaline  earths,  even 
AlCls+Aq,  dissolve  the  metal.  Insol.  in 
alum,  or  in  NaCl+Aq,  but  sol.  in  alum+ 
NaCl+Aq.  (Tissier,  C.  R.  41.  362);  sol.  in 
NaCl+Aq  (Deville,  A.  ch.  (3)  43.  14);  sol. 
in  neutral  FeCl3+Aq  in  vacuo.  (Weeren, 
B.  24.  1798.)  Violently  attacked  by  CuCl2  + 
Aq.  (Tommasi,  Bull.  Soc.  (2)  37.  443.) 

Rapidly  sol.  in  K2S2O8+Aq,  more  slowly 
sol.  in  (NH4),S,O8+Aq.  (Levi,  Gazz.  ch.  it. 
1908,  38.  (1)  583.) 

Attacked  by  (NH4)3PO4+Aq.  SI.  attacked 
by  NaNO3+Aq  or  KNO3+Aq  at  100°. 
(Smith,  J.  Soc.  Chem.  Ind.  1904,  23.  475.) 

Not  affected  by  NH4NO3+Aq.  (Hodgkin- 
son,  C.  N.  1904,  90.  142.) 

Attacked  by  POC13  at  100°.  (Renitzer,  B. 
13.  845.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  826.) 

Insol.  in  liquid  CO2.  (Biichner,  Z.  phys. 
Ch.  1906,  64.  674.) 

Attacked  by  NOC1.  (Sudborough,  Chem. 
Soc.  1891,  59.  659. 

92  %alcohol  attacks  Al  less  than  H2O.  Pure 
Al  is  attacked  less  than  commercial.  (Hugou- 
nenq,  J.  Pharm.  1895,  (6)  1.  537.) 

Sol.  in  organic  acids  containing  chlorides. 
(Smith,  J.  Soc.  Chem.  Ind.  1904,  23.  475.) 

Acetic,  tartaric  and  citric  acids  attack  Al 
only  at  first.  Metal  is  covered  by  layer  of 
hydrox'de  but  on  addition  of  haloid  salts, 
gradual  solution  ensues.  (Ditte,  C.  R.  1898, 
127.  919.) 

Not  attacked  bv  sugar+Aq.  (Klein,  C.  R. 
102.  1170.) 

Aluminum  arsenide. 

Decomp.  by  H->O  with  evolution  of  AsH3. 
(Wohler,  Pogg.  11.  160.) 

Decomp.  by  H2O.  (Fonzes-Diacon,  C.  R. 
1900,  130.  1315.) 

Aluminum  boride,  A12B4. 

Very  slowly  sol.  in  hot  cone.  HCl+Aq,  and 
hot  NaOH+Aq,  but  easily  in  moderately 
strong  warm  HNO3+Aq.  (Hampe,  A.  183. 

A12B24.  Not  attacked  by  HC1,  or  KOH  + 
Aq.  Scarcely  attacked  by  boiling  H2SO4. 
Hot  cone.  HNO3+Aq  dissolves  gradually  but 
completely.  (Hampe,  1.  c.) 

Aluminum  borocarbide,  A13C2B48. 

Insol.  in  H2O,  HCl+Aq,  H2SO4+Aq,  or 


ALUMINUM  CHLORIDE 


KOH+Aq;  slowly  sol.  in  hot  cone.  HNO3+ 
Aq.    (Hampe,  1.  c.) 

Aluminum  bromide,  AlBr3. 

Anhydrous.  Dissolved  by  H2O  with  great 
violence  and  evolution  of  much  heat.  Very 
sol.  in  alcohol.  More  sol.  in  CS2  than  A1I3. 
(Weber,  Pogg.  103.  264.) 

Sol.  in  SOC12.  (Besson,  C.  R.  1896,  123. 
884.) 

Sol.  in  C2H5Br.  (Plotnikoff,  G.  C.  1902, 
II.  617.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328);  (Eidmann,  C.  C.  1899,  II.  1014.) 

Solubility  of  AlBr3  in  organic  liquids. 


Aluminum  perbromide  carbon  bisulphide, 
AlBr3,  Br4,  CS2. 

Sol.  in  ether,  ethyl  bromide,  ethylene  brom- 
ide and  benzene;  decomp.  by  H2O.  (Plot- 
nikoff,  J.  Russ.  phys.  Chem.  Soc.  1901,  33. 
91;  C.  C.  1901,  I.  1193.) 

2AlBr3,  Br4,  CS2.  Sol.  in  ether  and  benzene; 
insol.  in  petroleum  ether.  (Plotnikoff,  I.  c.) 

Aluminum  bromochloride,  AlCl2Br. 

Deliquescent .  Somewhat  less  violently  dis- 
solved by  H2O  than  is  AlBr3.  (v.  Bartal, 
Z.  anorg.  1907,  55.  154.) 

+6H2O.  Deliquescent.  Sol.  in  H20  with- 
out evolution  of  heat.  (v.  Bartal,  Z.  anorg. 


Solvent 

t° 

,8 

o 

t° 

|8 

t° 

!§ 

JLJ7LM,    UU.     J.UU.  ) 

Aluminum  carbide,  A14C3. 

^  £ 

^  «3 

Decomp.  by  fused  KOH  at  100°;  insol.  in 

a 

a 

fuming  HNO3  in  the  cold;  decomp.  by  H2O, 
and  dil.  acids.    (Moissan,  Bull.  Soc.  1894,  (3) 
11.  1012;  C.  R.  1894,  119.  16-20.) 
Insol.  in  acetone.    (Naumann,  B.  1904,  37. 
4328.) 

48° 
45 
42 

0 
8.5 
13.8 

130° 
140 
142 

43.2 
48.4 
50 

50° 
38 
50 

66.0 
67.2 
70.7 

38 

18.3 

140 

52.1 

60 

74.2 

50 

21 

130 

54.5 

70 

78.3 

Aluminum  chloride,  basic,  Al6Oi4Hi0,  HC1. 

Benzo- 

60 

23.4 

120 

56.7 

80 

83.3 

Easily  sol.  in  H2O.     (Schlumberger,  Bull. 

phenone 

70 

25.7 

110 

58.6 

85 

86.7 

Soc.  1895,  (3)  13.  56.) 

80 
90 

28.1 
30.6 

100 
90 

60.3 
61.7 

90 
93 

90.7 

94.8 

Aluminum  chloride,  A1C13. 

100 

33.4 

80 

62.9 

96 

100 

Anhydrous.     Very  deliquescent.      Sol.  in 

110 

36.3 

70 

64.1 

H2O  with  a  hissing  noise  and  evolution  of 

120 

39.6 

60 

65.1 

heat.    Solution  of  A1C13  in  H20  loses  HC1  on 

evaporation,  and  A1C13  is  finally  wholly  con- 

10° 

o 

20° 

33.9 

70° 

72.7 

verted  into  A12O3. 

6 

8.4 

30 

40  1 

80 

82  3 

Sol.  in  1.432  pts.  H2O  at  15°.    (Gerlach.) 

Ethylene 

2 

40 

47.2 

90 

92.2 

AlCl3+Aq  containing  19.15  %  A1C13  boils 

bromide 

2 
10 

22.9 

28.4 

50 
60 

55.1 
63.6 

96 

100 

at  103.4°;  AlCl3+Aq  containing  38.3  %  A1C13 
boils  at  112.8°.    (Gerlach.) 

Sp.  gr.  of  AlCl3+Aq  at  15°. 

—0.5° 

0 

85° 

47 

40° 

72.6 

c 

Sp.  gr. 

C1 

Sp.  gr. 

2  5 

6  5 

90 

50  8 

60 

79.4 

/o 

—  5 

13.0 

80 

52.8 

70 

83.9 

1 

1.0072 

22 

1  .  1709 

Benzoyl 

10 

17.4 

60 

56 

80 

89.2 

2 

.0144 

23 

1  .  1795 

chloride 

30 

24.6 

40 

59.5 

90 

95.8 

3 

.0216 

24 

1  .  1881 

50 

31.8 

20 

63.1 

96 

100 

4 

.0289 

25 

1  .  1968 

70 

40 

7 

65,5 

5 

.0361 

26 

1.2058 

80 

44.3 

20 

67.9 

6 

.0435 

27 

1.2149 

(Menschutkin,    Ann.    Inst.    Pol.     P.-le-Gr., 

7 
8 

.0510 
.0585 

28 
29 

1  .  2241 
1.2331 

13.  1.) 

9 

.0659 

30 

1.2422 

+6H2O.    Very  sol.  in  H2O.                  W 
+15H2O.    (Panfiloff,  J.  B.  1895.  785.) 

10 
11 
12 

.0734 
.0812 
.0890 

31 
32 
33 

1.2518 
1.2615 
1.2711 

Aluminum  antimony  bromide,  2AlBr3,  5SbBr5 
+24H2O. 

13 
14 

.0968 
.1047 

34 
35 

1.2808 
1.2905 

Hygroscopic.     Decomp.  by  H2O.     (Wein- 
land,  B.  1903,  36.  258.) 

15 
16 
17 

.1125 
.1207 
1.1290 

36 
37 

38 

1.3007 
1.3109 
1.3211 

Aluminum  potassium  bromide,  AlBr3,  KBr. 

18 

1.1372 

39 

1.3313 

Sol.  in  H2O.    (Weber,  Pogg.  103.  267.) 

19 

1.1455 

40 

1.3415 

Aluminum  bromide  ammonia,  AlBr3,  zNH3. 

20 
21 

1  .  1537 
1  .  1632 

41 

1.3522 

Decomp.   by   H2O.      (Weber,    Pogg.    103. 

267.) 

(Gerlach,  Z.  anal.  8.  281.) 

ALUMINUM   AMMONIUM   CHLORIDE 


Sp.  gr.  at  20°  of  AlCl3+Aq  containing  mg. 
mols.  A1C13  per  liter. 


M. 

Sp.  gr. 

0.01 

1.00104 

0.025 

1.00282 

0.05 

1.00588 

0.075 

1.00870 

0.10 

1.01158 

0.25 

1.02911 

0.55 

1.05706 

1.0 

1.11054 

1.5 

1.16308 

2.0 

1.21378 

(Jones  &  Pearce,  Am.  Ch.  J.  1907,  38.  726.) 

Sol.  in  1  pt.  strong  alcohol  at  12.5°  (Wen- 
zel);  easily  sol.  in  ether;  si.  sol.  in  CS2;  insol. 
in  ligroine  or  benzene. 

Difficultly  sol.  in  AsBr3.  (Walden,  Z. 
anorg.  1902,  29.  374.) 

Sol.  in  AlBr3.  (Isbekow,  Z.  anorg.  1913, 
84.  26.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  826.) 

Insol.  in  CS2  at  ord.  temp.  (Arctowski,  Z. 
anorg.  1894,  6.  257.) 

Sol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1369.) 

Difficultly  sol.  in  acetone.  (Naumann,  B. 
1904,  37.  4328.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

Insol.  in  methylal.  (Eidmann,  C.  C.  1899, 
II.  1014.) 

Solubility  of  A1C13  in  organic  liquids. 


<*§ 

»1 

|2 

Solvent 

t° 

i| 

t° 

^ 

t° 

48° 
44 

0 

8.5 

130° 
125 

43.2 

48.4 

130° 
140 

66.0 
67.2 

39.5 

13.8 

120 

50 

150 

70.7 

50 

18.3 

110 

52.1 

160 

74.2 

60 

21. 

100 

54.5 

170 

78.3 

Benzo- 

70 

23.4 

90 

56.7 

180 

83.3 

phenone 

80 

25.7 

80 

58.6 

185 

86.7 

90 

28.1 

70 

60.3 

190 

90.7 

100 

30.6 

60 

61.7 

192 

94.8 

110 

33.4 

80 

62.9 

194 

100 

120 

36.3 

100 

64.1 

125 

39.6 

120 

65.1 

-0.5° 

0 

60° 

33.0 

80° 

52.9 

-4 

7.9 

70 

37.5 

70 

55.1 

Benzoyl 

-7.5 

12.7 

80 

42.2 

60 

57.2 

chloride 

0 

14.1 

90 

47.1 

40 

61.0 

20 

18.8 

93 

48.7 

40 

25.0 

90 

50.6 

(Menschutkin,    Ann.    Inst.    Pol.    P.-le-Gr.. 

13.  1.) 

+6H2O.  Very  deliquescent;  very  sol.  in 
H2O.  Sol.  in  0.25  pt.  H2O.  (Thomson.) 

Sol.  in  2  pts.  abs.  alcohol  at  ordinary  temp., 
and  1.5  pts.  at  b.-pt.  (Thomson.) 

Completely  insol.  in  a  solution  of  ether  in 
H2O  sat.  with  HC1.  (Havens,  Am.  J.  Sci. 
1898,  (4)  6.  46. 

Aluminum  ammonium  chloride,  Aids,  NH4C1. 
(Baud,  A.  ch.  1904,  (8)  1.  46.) 
Aluminum  antimony  chloride. 
See  Chlorantimonate,  aluminum. 

Aluminum  barium  chloride,  2A1C13,  BaCl2. 
(Baud,  C.  R.  1901,  133.  869.) 

Aluminum  calcium  chloride,  basic. 

3CaO,  CaCl2,  A1203+10H20.  (Steinmetz, 
Z.  phys.  Ch.  1905,  62.  466.) 

lOCaO,  CaCl2,  6A12O3.  Slowly  decomp.  by 
boiling  H2O.  (Gorgeu,  Bull.  Soc.  1887,  (2) 
48.  51.) 

Aluminum  calcium  chloride,  4A1C13,  SCaCU 

(Baud,  A.  ch.  1904,  (8)  1.  51.) 
Aluminum  nitrosyl  chloride,  A1C13,  NOC1. 

Deliquescent,  and  decomp.  by  H2O.  (Weber 
Fogg,  118.  471.) 

Aluminum  palladium  chloride,  A1C13,  PdCl2+ 

10H20. 
See  Chlorbpalladite,  aluminum. 

Aluminum  phosphorus  pentachloride,  A1C13, 

PC15. 
Decomp.  violently  by  H2O.    (Baudrimont.) 

Aluminum  phosphoryl  chloride,  A1C13,  POC13. 
Deliquescent.     Sol.  in  H2O  with  decomp. 
Sol.  in  warm  POC13,  from  which  it  separates 
on  cooling.    (Casselmann,  A.  98.  220.) 

Aluminum  platinum  chloride,  A1C13,  PtCl2  + 

15H2O. 
See  Chloroplatmite,  alumhium. 

Aluminum  potassium  chloride,  A1C13,  KC1. 

Slowly  deliquescent.  Sol.  in  H2O  with 
evolution  of  heat  and  decomp.  (Degen,  A. 
18.  332.) 

Alumhium  selenium  chloride,  2A1C13,  SeCl*. 

Sol.  in  H20  with  evolution  of  heat  'and 
separation  of  traces  of  selenium.  (Weber, 
Pogg.  104.  427.) 

Aluminum  sodium  chloride,  A1C13,  NaCl. 

Much  less  deliquescent  than  A1C13.  Sol.  in 
H2O  with  evolution  of  heat.  Upon  evaporat- 
ing, NaCl  crystallises  out.  (Wohler.) 

Aluminum  strontium  chloride,  4A1C13,  3SrCl2. 

(Baud,  A.  ch.  1909,  (8)  1.  52.) 
Aluminum  sulphur  chloride,  2A1C13,  SC14. 

Decomp.  by  H2O  with  evolution  of  much 


ALUMINUM   MAGNESIUM   FLUORIDE 


9 


heat  and  separation  of  some  sulphur.    (Weber 
Pogg,  104.  421.) 

A1C13,SC14.  Decomp.  by  H2O.  (Ruff,  B 
1901,  34. 1757.) 

Aluminum  tellurium  chloride,  2A1C13,  TeCl4. 
Very  sol.  in  dil.  H2SO4 + Aq.    (Weber,  J.  pr 
76.  313.) 

Aluminum  chloride  ammonia,  A1C13,  NH3. 

Sol.  in  H2O.    (Rose,  Pogg,  24.  248.) 

Completely  sol.  in  H,O.  (Baud,  C.  R. 
1901,  132.  135.) 

A1C13,  2NH3.  Very  hygroscopic.  (Still- 
man,  Am.  Ch.  J.  1895,  17.  750.) 

A1C18,  3NH3.    Decomp.  by  H2O. 

AlClj,  5NH3.  M.  pt.  380°.  (Baud,  C.  R. 
1901,  132.  135.) 

A1C13,  6NH3.  Decomp.  by  H2O.  (Still- 
man,  Am.  Ch  J.  1895,  17.  752.)  Somewhat 
hygroscopic.  (Baud,  C.  R.  1901,  132.  135.) 

Aluminum  chloride  nitric  oxide,  [2A1C13,  NO. 
Very  hygroscopic.    Decomp.  rapidly  in  the 
air.     Sol.  in  KOH+Aq.     (Thomas,   C.   R. 
1895,  121.  130.) 

Aluminum  chloride  phosphine,  3A1C13,  PH3. 
Decomp.  by  H2O  or  NH4OH+Aq.    (Rose 
Pogg,  24.  2950 

Aluminum  chloride  hydrogen  sulphide. 

Deliquescent.  Decomp.  by  H2O  or  NH4OH 
+Aq.  (Wohler.) 

Aluminum  chloride  sulphur  dioxide,  A1C13, 
SO2. 

Decomp.  by  H2O,  alcohol,  or  benzene. 
(Adrianowski,  B.  12.  688.) 

2A1C13,  SO2.    (Baud,  A.  ch.  1904,  (8)  1.  32.) 

Aluminum  cobalt,  Co3Al3. 

Sol.  in  strong  acids.    (Brunck,  B.  1901,  34. 

2734.) 

Aluminum  copper,  Cu4Al9. 

Sol.  in  aqua  regia;  decomp.  by  HC1. 
(Brunck,  B.  1901,  34.  2733.) 

Aluminum  fluoride,  A1F3. 

Anhydrous.  Not  attacked  by  H2O  or  acids, 
and  only  very  slightly  by  boiling  cone.  H2SO4. 
Insol.  in  boiling  KOH+Aq.  (Deville,  C.  R. 
42.  49.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

+  ^H2O.  Insol.  in  H2O.  SI.  sol.  in  HF. 
(Baud,  C.  R.  1902,  135.  1104.) 

-f-H2O.  Completely  but  only  sparingly  sol. 
in  H2O.  (Mazzuchelli,  Real.  Ac.  Line.  1907, 
(5)  16,  I.  775;  Chem.  Soc.  1907,  92,  (2).  549.) 

+3^H2O.  Two  modifications:  (1)  Easily 
sol.  in  H2O.  Sol.  in  HF.  (2)  Insol.  in  H2O. 
SI.  sol.  in  HF.  (Baud,  C.  R.  1902,  135.  1104.) 


-f  7H2O.  Sol.  in  H2O.  (Deville,  A.  ch.  (3) 
61.  329.) 

Min.  Fluellile. 

+83/2H20.  Very  efflorescent.  Sat.  solu- 
tion contains  3.85  g.  A1F3  per  100  g.  at  11° 
and  1.2  g.  at  -  0.2°.  (Mazzucchelli,  Real.  Ac. 
Line.  1907,  (5)  16,  I.  775;  Chem.  Soc.  1907, 
(2),  92.  549.) 

Aluminum  hydrogen  fluoride,  3A1F3,  2HF  + 
5H2O. 

Sol.  in  H20;  precipitated  by  alcohol. 
(Deville.) 

2A1F3,  HF+5H2O.  (Deville,  A.  ch.  (6)  61. 
o29.) 

Aluminum  ammonium  fluoride,  A1F3,  NH4F. 

Somewhat  sol.  in  H2O;  insol.  in  H2O  con- 
taining NH4OH  or  NH4F.  (Berzelius,  Pogg. 
1.  45.) 

A1F3,  2NH4F+1.5H20.  Sol.  in  100  pts. 
H2O  at  16°.  (Baud,  C.  R.  1902,  135.  1338  ) 

A1F3,  3NH4F.  Nearly  insol.  in  H2O;  easily 
sol.  in  dil.  acids.  (Petersen,  J.  pr.  (2)  40.  35.) 

Quite  easily  sol.  in  H2O,  but  insol.  in 
NH4F+Aq.  (Helmholt,  Z.  anorg.  3.  129.) 

Aluminum  barium  fluoride. 

Apparently  not  obtained  in  pure  state. 
(Roder.) 

Aluminum  calcium  fluoride,  A1F3,  CaF2-f-H2O. 
Min.  Evigtokite. 

Aluminum   calcium   sodium   fluoride,    A1F3, 

CaF2,  NaF+H20. 
Min.  Pachnolite. 

Aluminum  cobaltous  fluoride,  A1F3,  CoF2  + 
7H20. 

Sol.  in  dil.  HF+Aq.  (Weinland,  Z.  anorg. 
1899,  22.  272.) 

Aluminum  cupric  fluoride,  2A1F3,  CuF2. 

Very  slowly  but  completely  sol.  in  H2O. 
(Berzelius.) 

A1F3  2CuF2  +  llH2O.  Sol.  in  dil.  HF+Aq. 
(Weinland,  Z.  anorg.  1899,  22.  272-76.) 

2A1F3,  3CuF2  +  18H2O.  Sol.  in  dil.  HF  + 
Aq.  (Weinland.) 

Aluminum  cupric  hydrogen  fluoride,   A1F3, 

CuF2,  HF+8H20. 

Efflorescent  in  the  air.  Sol.  in  dil.  HF  +  Aq. 
(Weinland,  Z.  anorg.  1899,  22.  272.) 

Aluminum    iron     (ferrous)    fluoride,    A1F3, 

FeF2+7H2O. 

SI.  sol.  in  dil.  HF+Aq.  (Weinland,  Z. 
anorg.  1899,  22.  270.) 

Aluminum  lithium  fluoride. 
Insol.  in  H2O.    (Berzelius.) 

Aluminum  magnesium  fluoride. 
2A1F3,  MgF2  (?).    (Roder.) 


10 


ALUMINUM   NICKEL   FLUORIDE 


Aluminum  nickel  fluoride,  A1F3,  NiF2+7H2O. 
SI.  sol.  in  dil.  HF+Aq.     (Weinland,  Z. 
anorg.  1899,  22.  271.) 

Aluminum  potassium  fluoride,  A1F3,  3KF. 

Very  si.  sol.  in  acid  solutions,  and  still  less 
in  H2O.  (Gay-Lussac  and  Thenard.) 

A1F3,  2KF.    As  above. 

Aluminum  silicon  fluoride. 
See  Fluosilicate,  aluminum. 

Aluminum  sodium  fluoride. 

2A1F3,  3NaF.    Min.  Chiolite. 

A1F3,  2NaF.    Min.  Chodneffite. 

A1F3,  3NaF.  Min.  Cryolite.  SI.  sol.  in 
H2O.  Insol.  in  HCl+Aq.  Decomp.  by 
H2SO4,  or  by  boiling  with  NaOH+Aq. 

Aluminum  strontium  fluoride. 
As  the  Ba  salt.    (Roder.) 

Aluminum  thallous  fluoride,  2A1F3,  3T1F. 

Ppt.  SI.  sol.  in  H2O.  (Ephraim,  Z.  anorg. 
1909,  61.  243.) 

Aluminum  zinc  fluoride,  A1F3,  ZnF2+7H2O. 

Sol.  in  dil.  HF+Aq.  (Weinland,  Z.  anorg. 
1899,  22.  272.) 

2A1F3,  ZnF2.  Slowly  but  completely  sol. 
in  H2O.  (Berzelius.) 

Aluminum  hydroxide,   A12O3,    H2O 
=A1202(OH)2. 

Dehydrated  by  cone,  acids,  without  dissolv- 
ing. (Becquerel,  C.  R.,  67.  108.) 

Min.  Diaspore.  Insol.  in  HCl+Aq,  and 
not  attacked  by  boiling  cone.  H2SO4,  unless 
it  has  been  ignited. 

A12O3,  2H2O=A12O(OH)4.  Pptd.  Al  hy- 
droxide, when  boiled  twenty  hours  with  H2O 
is  insol.  in  acids  and  alkalies,  and  has  the 
above  composition.  (St.  Gilles,  A.  ch.  (3) 
46.  57.) 

Min.  Bauxite. 

Soluble  modifications — -(a)  M eta-aluminum 
hydroxide  From  basic  Al  acetate.  Sol.  in 
H2O  and  more  readily  in  HC2H3O?.  The 
aqueous  solution  is  coagulated  by  traces  oi 
alkalies,  many  acids,  and  salts,  while  other 
acids  and  salts  have  no  effect .  Thus,  1  pt 
H2SO4  in  1000  pts.  H2O,  added  to  7000  pts.  of 
above  solution  containing  20  pts.  A12O3,  con- 
verts the  liquid  into  a  nearly  solid  mass 
Citric,  tartaric,  oxalic,  chromic,  molybdic 
racemic,  suberic,  salicylic,  benzoic,  gallic 
lactic,  cinnamic,  butyric,  valeric,  camphoric 
picric,  uric,  meconic,  comenic,  and  hemipini< 
acids  act  in  the  same  way.  HC1  and  HNO; 
have  far  less  action,  600  mols.  being  necessary 
to  produce  the  same  effect  as  1  mol.  H2SO4 
while  acetic,  formic,  boric,  arsenious,  pyro- 


meconic,  and  opianic  acids  do  not  coagulate 
he  solution,  except  when  moderately  cone. 
_  pt.  KOH  in  1000  pts.  H2O  coagulates  9000 
pts.  of  the  solution.  NaOH,  NH4OH,  and 
Ua(OH)2  have  the  same  effect. 

The  solution  is  not  coagulated  by  acetates, 
unless  added  in  large  quantity,  and  even 
then  the  ppt.  is  redissolved  when  treated  with 
32O  Nitrates  and  chlorides  coagulate  with 
difficulty;  Na2SO4,  MgSO4,  and  CaSO4+Aq, 
lowever,  have  as  strong  an  action  as  a  liquid 
containing  the  same  amount  of  H2SO4.  A 
;easpoonful  of  the  solution  introduced  into 
;he  mouth  solidifies  at  once  from  the  action 
of  the  saliva.  The  ppt.  formed  by  acids  is 
not  sol.  in  an  ecessx  of  the  acid,  but  by  the 
ong  continued  action  of  cone.  H2S04,  espe- 
cially if  hot,  the  ppt.  is  dissolved;  boiling 
cone.  HCl+Aq  also  dissolves  it,  but  less  read- 
ily than  H2S04.  The  ppt.  is  sol.  in  boiling 
cone.  KOH+Aq.  The  residue,  when  the 
solution  is  evaporated  at  100°,  has  composi- 
tion A12O3,  2H20,  and  is  insol.  in  acids. 
(Crum,  Chem.  Soc.  6.  225.) 

(b)  By  Dialysis.  Sol.  in  H2O,  from  which 
it  is  separated  by  extremely  small  amounts  of 
various  substances,  as  acids,  ammonia,  salts 
(especially  K2S04),  caramel,  etc.  An  excess 
of  acid  dissolves  the  coagulum.  If  the  solu- 
tion contains  0.5%  A12O3  or  less,  it  may  be 
boiled  without  change,  but  the  hydroxide 
separates  out  suddenly  when  it  is  reduced  to 
^2  its  vol.,  and  even  very  dil.  solutions  gela- 
tinise spontaneously  in  a  few  days.  The 
solution  is  not  coagulated  by  alcohol  or  sugar. 
(Graham,  A.  121.  41.) 

A12O3,3H2O=A1(OH)3.  Crystallised.  Diffi- 
cultly sol.  in  acids  and  alkalies.  (Cossa,  N. 
Cim.  (2)  3.  228.)  Insol.  in  boiling  HCl+Aq. 
(Wohler,  A.  113.  249.)  SI.  sol.  in  KOH+Aq; 
nearly  insol.  in  cold  H2SO4,  HC1,  HNO3+Aq; 
verv  slowly  sol.  in  hot  HCl+Aq,  more  readily 
in  hot  H2SO4.  (v.  Bonsdorff,  Pogg.  27.  275.) 

a-modification.  Unstable.  Changes  into 
jS-modification.  Sol.  in  N-H2SO4  at  ord. 
temp.  Sol.  in  N-NaOH  and  in  hot  NaOH  of 
concentration  5Na2O,  100H2O.  (Russ,  Z. 
anorg.  1904,  41.  226.) 

/3-modification.  Insol.  in  N-H2SO4  at  ord. 
temp.  Difficulty  sol.  in  warm  N-NaOH,  but 
easily  sol.  in  hot  NaOH  of  concentration 
5Na2O,  100H2O.  Its  solubility  in  NaOH  in- 
creases with  increase  in  concentration  of  the 
hydroxyl  ions.  (Russ.) 

5-modification.  Easily  sol.  in  cone.  H2SO4; 
only  si.  sol.  in  HC1,  HNO3  or  acetic  acids,  or 
in  alkali +Aq.  (Tommasi,  C.  C.  1905,  II. 
605.) 

Min.  Gibbsite.  Sol.  in  HCl+Aq,  and  dil. 
H2SO4+Aq.  Readily  sol.  in  cone.  KOH,  and 
NaOH+Aq. 

Precipitated.  Completely  insol.  in  H2O  or 
H2CO3+Aq.  Easily  sol.  in  acids  when  freshly 
pptd.,  but  solubility  diminishes  on  standing 

Easily  sol.  in  KOH  or  NaOH+Aq.  (Son- 
nenschein.) 


ALUMINUM   MERCURIC  IODIDE 


11 


Herz  (Z.  anorg.  25.  155)  found  that  alum- 
inum hydroxide  which  has  been  dried  in  a 
vacuum  dessicator  requires  for  solution  in 
NaOH-j-Aq.  3  atoms  Na  to  1  atom  Al. 
Slade  (Z.  Elektrochem.  1911,  17.  261)  was 
unable  to  obtain  this  result .  Herz  says  Slade' s 
error  is  due  to  insufficient  shaking  of  the  solu- 
tion. (Herz,  Z.  Elektrochem.  1911,  17.  403.) 

New  solubility  determinations  verify  the 
statement  of  Herz  (Z.  anorg.  25,  155)  that  the 
solubility  of  A1(OH)3  in  NaOH+Aq  is  pro- 
portional to  the  concentration  of  NaOH. 
They  do  not,  however,  verify  his  statement 
that  the  ratio  Na  :  Al  in  the  solutions  is  al- 
ways 3  :  1,  for  the  author  finds  that  the  ratio 
Na  :  Al  varies  from  2  :  1  to  10  :  1  depending 
on  the  conditions  of  precipitation  and  the 
method  and  duration  of  drying  of  the  A1(OH)3. 
(Slade,  Z.  Elektrochem,  1912,  18.  1.) 

SI.  sol.  in  NH4OH+Aq  when  freshly  pptd., 
but  presence  of  NH4  salts  diminish  its  solu- 
bility, and  it  separates  out  completely  after 
long  standing.  (Fresenius.) 

Somewhat  sol.  in  NH4OH+Aq,  the  more 
readily  the  larger  the  vol.  of  H2O.  Somewhat 
sol.  in  (NH4)2CO3+Aq,  but  less  than  in 
NH4OH+Aq.  SI.  sol.  in  dil.  NH4Cl+Aq, 
unless  that  salt  be  in  large  excess.  It  is  finally 
wholly  pptd.  if  allowed  to  stand  several  days. 

18752  pts.  NH4OH+Aq  (4  %  NH4OH)  dis- 
solve an  amt.  of  A1(OH)3  corresponding  to  one 
pt.  A12O3;  NH4C1  prevents  this  solubility  al- 
most completely.  (Hanamann,  Pharm.  Vier- 
telj.  12.  527.)  r 

A1(OH)3,  prepared  by  ppt.  of  a  solution  of 
A1(NO8)8  with  NH4OH,  filtered  and  washed, 
is  insol.  in  NH4OH+Aq. 

A1(OH)3  prepared  by  pptn.  of  a  solution  of 
potassium  aluminate  with  NH4C1,  is  sol.  in 
a  large  excess  of  NH4OH  if  this  is  added  to 
the  ppt.  at  once.  This  modification  which  is 
sol.  in  NH4OH  is  unstable  and  easily  goes 
over  into  the  modification  which  is  insol.  in 
NH4OH.  (Renz,  B.  1903,  36.  2751.) 

Cone.  (NH4)2CO3+Aq  does  not  dissolve 
A1(OH)3,  and  not  a  trace  is  dissolved  by  boiling 
cone.  NH4Cl+Aq.  (Weeren,  Pogg.  92.  97.) 

With  NH4F+Aq,  it  forms  a  double  salt, 
A1F3,  3NH4F,  which  is  sol.  in  H2O,  but  not  in 
NH4F+Aq.  (Helmholt,  Z.  anorg.  3.  127.) 

Insol.  in  (NH4)2S+Aq.  (Malaguti  and 
Durocher,  A.  ch.  (3)  17.  421.)  Fuchs  found, 
on  the  contrary,  that  it  is  not  wholly  insol.  in 
(NH4)2S+Aq.  (Fresenius,  Quant.) 

Insol.  in  FeCl3+Aq.    (Bechamp.) 

Determinations  of  the  solubility  of  alum- 
inum hydroxide  in  AlCl3+Aq  show  that  part 
goes  into  solution  to  form  a  compound,  while 
the  greater  part  is  in  the  colloidal  form. 
(Fischer,  Z.  anorg.  1904,  40.  46.) 

Only  si.  sol.  in  cone.  Al2(SO4)3+Aq,  but 
solubility  increases  with  decrease  in  concen- 
tration of  A12(SO4)3  until  it  reaches  a  maxi- 
mum at  a  concentration  of  32  %  A12(SO4)3 
at  20°,  28  %  at  40°,  and  38  %  at  60°.  With 
further  decrease  in  concentration  of  A12(SO4)3 


the  solubility  of  A1(OH)3  in  A12(SO4)3  dim- 
inishes. (Kremann,  C.  A.  1909.  2422.) 

Sol.  in  Ba(OH)2+Aq.    (Rose.) 

Sol.  in  boiling  Fe(NO3)3,  Cr(NO3)3, 
Bi(N03)3,  Hg(N03)2,  HgN03,  SnCl2,  and 
SbCl3+Aq.  (Persoz.) 

Insol.  in  HCN  or  cold  KCN+Aq;  but  si. 
sol.  in  hot  KCN+Aq.  (Rose.) 

Insol.  in  KC2H3O2+Aq.    (Osann,  1821.) 

When  moist,  sol.  in  H2SO3+Aq,  from  which 
it  is  repptd.  on  boiling.  (Berthier,  A.  ch.  (3) 
7.  76.) 

Somewhat  sol.  in  NaC2H3O2+Aq.  (Mer- 
cer.) 

Not  pptd.  by  NH4OH+Aq  in  presence  of 
Na  citrate.  (Spiller.) 

Sol.  in  ethyl  amine,  amyl  amine,  sinkaline, 
ethyl  picoline  hydroxide^  stibethylium  hy- 
droxide, triethyltoluenyl  ammonium  hydrox- 
ide+Aq.  (Friedlander.) 

Sol.  in  alkyl  amines.     (Renz,  B.  1903,  36. 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

Sol.  to  a  considerable  extent  in  K.>C4H4Oe+ 
Aq. 

Very  si.  sol.  in  cane  sugar +Aq.    (Ramsey.) 

Solubility  in  glycerine  +Aq  containing 
about  60  %  by  vol.  of  glycerine.  100  cc. 
of  the  solution  contain  0.25  g.  A12O3.  (Miiller, 
Z.  anorg.  1905,  43.  322.) 

A1203,  5H2O.  Insol.  in  H2O,  NH4OH  + 
Aq  and  alcohol.  Sol.  in  HC1  and  HNO3+ 
Aq.  (Zunino,  Gazz.  ch.  it.  1900,  30  (1). 
194.) 

Al6Oi4Hio,  "  Trialuminum  hydroxide." 

Not  sol.  in  cone,  acids  in  the  cold;  not  sol. 
in  KOH  (cold)  and  only  si.  sol.  in  hot  KOH. 
Characterized  by  its  solubility  in  exactly  one 
mol.  dil.  HC1.  Dil.  solutions  do  not  gelatinize 
even  on  long  standing.  Cone,  solution  of 
NH4C1  and  other  salts  cause  ppt.  which  re- 
dissolves  on  addition  of  H2O. 

Alkalies  and  alkali  carbonates  decomp.  the 
salt  with  HC1  and  ppt.  trialuminium  hy- 
droxide. H2SO4  and  sol.  sulphates  give  insol. 
compds.  with  the  hydrate.  HNO3  like  HC1 
gives  soluble  compds.  with  the  hydrate. 
(Structural  formula  given.)  (Schlumberger, 
Bull.  Soc.  1895,  (5)  13.  41-65;  C.  C.  1895,  I. 
421.) 

Aluminum  iodide,  A1I3. 

Anhydrous.  Fumes  on  air  and  deliquesces. 
Sol.  in  H20  with  evolution  of  much  heat.  Sol. 
in  CS2  and  crystallizes  from  the  hot  sat.  solu- 
tion on  cooling.  (Weber.)  Sol.  in  alcohol 
(Weber) ;  ether  and  tetrachlormethane.  (Gus- 
tavson.) 

Sol.  in  AlBr3.  (Isbekow,  Z.  anorg.  1913, 
84.  26.) 

+6H2O.    Very  sol.  in  H2O. 

Aluminum  mercuric  iodide,  A1I3,  HgI2  -f  8H2O. 
Very  deliquescent;  sol.  in  H2O  without  de- 
comp.   (Duboin,  C.  R.  1908,  146.  1028.) 


12 


ALUMINUM  POTASSIUM  IODIDE 


Aluminum  potassium  iodide,  A1I3,  KI. 

Sol  in  H2O  with  evolution  of  much  heat. 
(Weber,  Pogg.  101.  469.) 

Aluminum  iodide  ammonia,  A1I3,  3NH3. 
Decomp.  by  H2O.    (Weber,  Pogg.  103. 263.) 

Aluminum  iodide  mercuric  oxyiodide,  2A1I3, 

HgO,  3HgI2+15H20. 
(Duboin,  C.  R.  1907,  145.  714.) 

Aluminum  iron,  FeAl3. 

Readily  sol.  in  strong  HNO3.  (Brunck,  B. 
1901,  34.  2734.) 

Aluminum  manganese,  Mn2Al7. 

Sol.  in  strong  HC1.  (Brunck,  B.  1901,  34. 
2735.) 

Aluminum  molybdenum,  Al4Mo. 

Easily  sol.  in  hot  HNO3  or  HC1.  (Wohler, 
A.  1860,  115.  103.) 

Al2Mo.    (Guillet,  C.  R.  1901,  133.  293.) 

AlMo.    (Guillet.) 

AlMo4.  Not  attacked  by  dil.  HCl+Aq. 
(Guillet.) 

AlMo20.  Not  attacked  by  HCl+Aq. 
(Guillet.) 

Aluminum  nickel,  Al3Ni. 

Sol.  in  strong  acids.  (Brunck,  B.  1901,  34. 
2734.) 

Aluminum  nitride,  A12N2. 

Slowly  attacked  by  hot  or  cold  H2O.  De- 
comp. by  acids  and  aqueous  solutions  of  the 
alkalies,  especially  when  they  are  concen- 
trated. (Mallet,  A.  186.  155.) 

Easily  decomp.  H2O  when  finely  powdered. 
(Rossil,  C.  R.  1895,  121.  942.) 

Decomp.  by  moist  air  and  bv  boiling  H2O 
and  by  alkalis+Aq.  (Franck,"  Ch.  Z.  1897, 
21.263. 

Aluminum  oxide,  Al2Os. 

Crystalline.  Min.  Corundum,  sapphire, 
ruby,  emery.  Insol.  in  acids. 

Amorphous.  Ignited  A12O3  is  insol.  in 
acids  except  that  it  dissolves  slowly  when 
heated  with  a  mixture  of  1  pt.  H2S04  and  1 
pt.  H2O.  (Berzelius.)  Slowly  sol. -in  boiling 
HCl+Aq.  '  (Rose,  Pogg.  52.  595.) 

Sol.  in  22  pts.  of  a  mixture  of  8  pts.  H2SO4 
and  1  pt.  H-jO.  (Mitscherlich.)  The  lower 
the  temperature  at  which  A12O3  has  been 
heated,  the  more  sol.  is  it  in  acids  and  alkalies. 

Solubility  in  (calcium  sucrate+ sugar)  + 
Aq. 

1  1.  solution  containing  418.6  g.  sugar  and 
34.3  g.  CaO  dissolves  1.35  g.  A12O3;  1  1.  solu- 
tion containing  296.5  g.  sugar  and  24.2  g. 
CaO  dissolves  0.32  g.  A12O3;  1  1.  solution  con- 
taining 174.4  g.  sugar  and  14.1  g.  CaO  dis- 


solves  0.19  g.  A12O3.  (Bodenbender,  J.  B. 
1865.  600.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

See  also  Aluminum  hydroxide. 

Aluminum  peroxide,  A12O3,  A12O4  +  10H2O. 
Ppt.;  sol.  in  acids  with  decomp.     (Terni, 
.  A.  1912.  3068.) 

Aluminum  oxybromide. 

Basic  aluminum  bromides  containing  three 
equivalents  or  less  of  A12O3  to  one  of  AlBr3 
are  sol.  in  H20.  Those  containing  more  than 
three  equivalents  are  insol.  (Ordway,  Am.  J. 
Sci.  (2)  26.  203.) 

Aluminum  oxychloride. 

Sol.  in  dil.  acids  or  alkalies.  Decomp.  by 
H2O.  (Hautefeuille  and  Perrey,  C.  R.  100. 
1220.) 

Basic  aluminum  chlorides  containing  two 
equivalents  or  less  of  A12O3  to  one  of  A1C13 
are  sol.  in  H20.  Those  containing  more  than 
two  equivalents  are  insol.  (Ordway.) 

A12O3,  3A1C13+3H2O.  (Tommasi,  Bull. 
Soc.  (2)  37.  443.) 

A1203,  8A1C13+3H20.    (Tommasi.) 

3A12O3,  A1C13+15H2O.    (Tommasi.) 

Aluminum  phosphide,  A13P. 

Unstable.    (Franck,  Ch.  Z.  1898,  22.  240.) 

A12P2.  Decomp.  by  H2O.  (Fonzes-Diacon, 
C.  R.  1900,  130.  1315.) 

Unstable.    (Franck,  Ch.  Z.  1898,  22.  240.) 

A13P7.  Decomp.  by  H2O  and  acids. 
(Franck.) 

A13P7.      Decomp.    by    H2O    and    acids. 

(Franck,  Ch.  Z.  1898," 22.  288.) 

A1SP3.  Unstable.  (Franck,  Ch.  Z.  1898, 
22.  240.) 

Aluminum  platinum,  Pt3Ali0. 

The  Al  is  dissolved  out  by  HC1.  (Brunck, 
B.  1901,  34.  2735.) 

Aluminum   selenide,   Al2Se3. 

Decomp.  by  H2O.  (Fonzes-Diacon,  C.  R. 
1900,  130.  1315.) 

Aluminum  silicide,  Al2Si4. 

More  easily  sol.  in  acids  than  Al.  (Winkler, 
J.  pr.  91.  193.) 

Aluminum  chromium  silicide,  Al2Cr4Si6. 

Insol.  in  hot  cone.  HC1,  HNO3,  H2SO4  and 
aquaregia.  Sol.  in  cold  HF  or  in  HF+HNO3. 
Sol.  in  molten  alkali.  Insol.  in  NaOH+Aq, 
KOCl+AqorfusedKClO3orKHSO4.  (Man- 
chot  and  Kieser,  A.  1904,  337,  356.) 

Al2Cr4Si8.  Insol.  in  hot  cone.  HC1,  HNO3, 
H2SO4  and  aqua  regia.  Sol.  in  HF  and  in 
molten  alkali.  (Manchot  and  Kieser,  A. 
1904,  337.  358.) 


AMIDOPHOSPHATE,  FERRIC 


13 


Aluminum  tungsten  silicide. 

Insol.  in  most  acids  and  aqua  regia.  Easily 
sol.  in  HF,  HNO3  and  in  molten  alkali.  Not 
attacked  by  dil.  NaOH+Aq.  (Manchot  and 
Kieser,  A.  1904,  337.  360.) 

Aluminum  vanadium  silicide,  Al2V8Sii3. 

Sol.  in  HF.  Not  attacked  by  hot  cone. 
HC1,  HN03,  H2SO4  or  aqua  regia.  Decomp. 
by  fusing  with  NaOH.  Stable  toward  fused 
KC103.  (Manchot,  A.  1907,  357.  134.) 

Aluminum  sulphide,  A1S. 

Decomp.  by  H2O.  Sol.  in  acids  and  alkalis. 
(Regelsberger,  Z.  Elektrochem,  1898,  4.  548.) 

A12S3.  Decomp.  in  moist  air  and  by  H2O. 
(Wohler.)  Insol.  in  acetone.  (Naumann,  B. 
1904,  37.  4328.) 

Aluminum  chromium  sulphide,  Al2S3,CrS. 

SI.  attacked  by  HCl+Aq.  Gradually  de- 
comp.  by  HNO3.  (Houdard,  C.  R.  1907, 
144.  1115.) 

Aluminum  magnesium  sulphide,  A12S3,  MgS. 
Decomp.    by    H20,    alcohol    and    acids. 
(Houdard,  C.  R.  1907,  144,  1116.) 

Aluminum  potassium  sulphide. 

Violently  decomposed  by  H20.  (St.  Claire 
Deville,  J.  pr.  71.  293.) 

Does  not  exist.    (Gratama,  R.  t.  c.  3.  4.) 

Aluminum  silver  sulphide,  5A12S3,  4Ag2S. 
(Cambi,  Real.  Ac.  Line.  (5)  21,  II.  838.) 

Aluminum  telluride. 

Decomp.  by  H2O.    (Wohler,  Pogg.  11. 160.) 

Aluminum  titanide,  Al4Ti. 

Not  attacked  by  H2O  or  by  cold  HN03. 
SI.  sol.  in  warm  HNO3.  Sol.  in  cold  cone. 
H2SO4  or  HC1.  Sol.  in  warm  KOH+Aq. 
(Levy,  A.  ch.  1902,  (6)  26.  449.) 

Sol.  in  HC1  and  in  aqua  regia.    (Guillet.) 

Al3Ti.  Sol.  in  hot  dil.  H2S04  and  in  hot 
KOH+aq.  Sol.  in  hot  cone,  acids.  (Man- 
chot, A.  1907,  357.  142.) 

Al3Ti2.  Aluminothermic  product  is  sol.  in 
HC1  and  aqua  regia.  (Guillet.) 

Aluminosulphuric      acid,     A12(SO4H)6+ 

7H20. 

Sol.  in  H2O  with  decomp.  into  A12(S04)3 
and  H2SO4.  (Silberberger,  M.  1904,  25.  222.) 

ZH'amide,  N2H4. 
See  Hydrazine. 

Amidochromic  acid. 

Amidochromates. 

Do  not  exist.    Those  described  by  Darm- 


stadter  and  Lowenthal  are  impure  bichro- 
mates.    (Wyrouboff,  Bull.  Soc.  1894,  (3)  11. 
3;  C.  C. 


845-53; 


1894,  II.  610.) 


Ammonium  amidochromate,  (NH4)NH2CrO3. 

Very  sol.  in  H2O.  (Lowenthal,  Z.  anorg. 
1894,  6.  363.) 

Is  ammonium  dichromate.  (Wyrouboff, 
Bull.  Soc.  (3)  11.  845.) 

Lithium  amidochromate,  LiNH2CrO3. 

Very  sol.  in  H2O  and  acids.  (Lowenthal, 
Z.  anorg.  1894,  6.  364.) 

Potassium  amidochromate,  KCrO3NH2. 

Sol.  only  in  H2O.  Sat.  solution  in  H2O 
contains  13  %  of  the  salt.  (Heintze,  J.  pr. 
(2)  4.  214.) 

Amidophosphoric     acid,     HPO3(NH2)  = 

PO(NH2)  (OH)2. 

Sol.  in  H2O,  but  decomp.  on  standing  or  by 
heat.  (Stokes,  Am.  Ch.  J.  16.  198.) 

Aluminum  amidophosphate. 
Ppt.    Sol.  in  NH4OH+Aq.    (Stokes.) 

Ammonium  amidophosphate, 

NH4HP03(NH2). 
Very  sol.  in  H2O.    (Stokes.) 

Barium  amidophosphate,  BaPO3(NH2)  +H2O. 

Very  si.  sol.  in  H2O.    (Stokes.) 

BaH2(PO3NH2)2+2MH2O.  Quite  diffi- 
cultly sol.  in  H2O.  (Stokes.) 

Calcium  amidophosphate,  CaP03(NH2). 

Much  less  sol.  in  H2O  than  Ba  salt. 
(Stokes.) 

CaH2(PO3NH2)2.  Much  less  sol.  in  H2O 
than  the  Ba  salt.  (Stokes.) 

Chromic  amidophosphate. 
Ppt.    Sol.inwarmNH4OH+Aq.    (Stokes.) 

Cobalt  amidophosphate. 
Neutral.    Ppt. 
Add.  SI.  sol.  in  H20;  sol.  in  NH4OH+Aq. 

Cupric  amidophosphate. 
Neutral.    SI.  sol.  in  H2O. 
Acid.    Nearly  insol.  in  H2O. 

Ferrous  amidophosphate. 

Neutral.  Sol.  in  much  H20,  and  in 
HC2H3O2,  or  NH4OH+Aq. 

Acid.  Nearly  insol.  in  H2O  or  NH4Cl+Aq. 
Sol.  in  NH4OH+Aq. 

Ferric  amidophosphate. 

Neutral.      Ppt.     Sol.  in  excess  of  alkali 


14 


AMIDOPHOSPHATE,  HYDROXYLAMINE 


amidophosphate  and  in  NH4OH + Aq.     Insol. 
in  HC2H3O2+Aq. 

Add.    As  the  neutral  salt. 

Hydroxylamine   amidophosphate, 

(NH30)HP03(NH2). 
SI.  sol.  in  H2O.    (Stokes.) 

Lithium  amidophosphate,  LiHPO3(NH2). 
SI.  sol.  in  H2O.    (Stokes.) 

Magnesium  amidophosphate,  MgPO3(NH2) 
+7H20. 

Very  si.  sol.  in  H2O;  quite  easily  sol.  in  dil. 
NH4Cl+Aq.  Sol.inHC2H3O2+Aq.  (Stokes.) 

MgH2(P03NH2)2  +  3MH2O.  Insol.  in 
NH4Cl+Aq.  (Stokes.) 

Manganese  amidophosphate. 
Neutral.    Ppt. 
Add.    SI.  sol.  in  H2O. 

Nickel  amidophosphate. 

Neutral.  Ppt.  Sol.  in  HC2H3O2  or 
NH4OH+Aq. 

Add.    SI.  sol.  in  H20. 

• 
Potassium  amidophosphate,  K2PO3(NH2). 

Very  sol.  in  H2O  and  not  decomp.  by  boil- 
ing. (Stokes.) 

KHPO3(NH2).  Easily  sol.  in  cold  H2O; 
insol.  in  alcohol.  (Stokes.) 

Silver  amidophosphate,  Ag2P03(NH2). 

Almost  insol.  in  H2O.  Sol.  in  HN03  or 
NH4OH+Aq. 

AgHPO3(NH2).  SI.  sol.  in  H20;  easily  sol. 
in  dil.  HNO3  or  HC2H302+Aq,  also  in 
NH4OH+Aq. 

Sodium  amidophosphate,  Na2P03(NH2). 

Not  deliquescent;  very  sol.  in  H2O;  pptd. 
from  aqueous  solution  by  alcohol.  (Stokes.) 

NaHPO8(NH2)+M(?)H2O.  Nearly  insol. 
in  cold,  and  decomp.  by  hot  H2O.  Insol.  in 
alcohol. 

Zinc  amidophosphate. 

Neutral.    Perceptibly  sol.  in  H2O. 

Add.  SI.  sol.  in  H2O;  sol.  in  NH4OH  or 
HC2H302+Aq. 

Diamidophosphoric  acid,  PO(NH2)2OH. 
Sol.  in  cold  H2O;  ahnost  insol.  in  alcohol; 
stable  in  the  air  but  decomp.  when  heated  and 
by  boiling  in  aq.  solution.  (Stokes,  Am.  Ch. 
J.  1894,  16.  130.) 

Barium  diamidophosphate,  [PO(NH2)2O]2Ba. 
Very  sol.  in  H2O;   insol.  in  alcohol;  aq. 
solution  decomp.  slowly.    (Stokes,  Am.  Ch. 
J.  1894,  16.  134.) 


Magnesium    diamidophosphate,    [PO(NH2)2 

0]2Mg. 
Sol,  in  H2O;  insol.  in  alcohol.    (Stokes.) 

Potassium  diamidophosphate,  PO(NH2)2OK. 
Sol.   in  H2O;  not   deliquescent;   insol.  in 
alcohol.    (Stokes.) 

Silver  diamidophosphate,  PO(NH2)2OAg. 

Very  stable;  insol.  in  H2O.  Very  sol.  in 
NH4OH+Aq.  (Stokes.) 

Sodium   cfo'amidophosphate,    PO(NH2)2ONa. 
Sol.   in  H20;  not  deliquescent;   insol.   in 
alcohol.     (Stokes.) 

Diamidofnhydroxylphosphoric  acid. 

Silver  diamidofnhydroxylphosphate, 

(AgO)3P(NHAg)2. 

(Stokes,  Am.  Ch.  J.  1894, 16.  147.) 

(AgO)3P(NH2)(NHAg).  Insol.  in  cold 
H2O.  (Stokes.) 

(AgO)3P(NH2)2.  Decomp.  by  cold  H20. 
(Stokes.) 

+2H2O.  Decomp.  by  boiling  H2O. 
(Stokes.) 

Amidoimidophosphoric  acid. 

Amidoheximidoheptaphosphoric  acid,  OH . 
PO .  (NHa)  [NH .  PO(OH)]5.NH; .  PO(OH)2 
=  P7N7015H16. 

Known  only  in  solution  in  H2O.  (Stokes, 
Am.  Ch.  J.  1898,  20.  758.) 

Silver   diamidopi/rimidophosphate, 

NH(PO.NH2.OAg)2. 

Almost  insol.  inH2O;  sol.  in  NH4OH+Aq. 
(Stokes,  Am.  Ch.  J.  1894,  16.  136.) 

Silver  amido^rimido  pentaphosphate, 

P6N5OnH3Ag9. 
Ppt.    (Stokes,  Am.  Ch.  J.  1898,  20.  752.) 

Silver  amido/ieximido^eptophosphate, 
P7N7015H9Ag7. 

Ppt.;  decomp.  by  acetic  acid.  (Stokes, 
Am.  Ch.  J.  1898,  20.  759.) 

Sodium   amidodiimidoZnphosphate, 

PO  oNa^NH-P°(°Na)2- 

<NHPO(ONa)NH2. 

=P3N307H4Na4+H20. 
Unstable;  sol.  in  H2O;    insol.  in  alcohol. 
(Stokes,  Am.  Ch.  J.  1896,  18.  643.) 

Sodium  axaldoheximidoheptaphosphsite. 

P7N7016H9Na7. 

Sol.  in  H2O;  pptd.  by  alcohol.  (Stokes, 
Am.  Ch.  J.  1898,  20.  758.) 


AMIDOSULPHONATE,  ZINC 


15 


Amidophosphimic  acid. 

Silver  amidophosphimate,P(NH)  NH2(OAg)2. 

Decomp.  by  heat;  decomp.  in  contact  with 
H2O.  (Stokes,  Am.  Ch.  J.  1894,  16.  139  ) 

(AgO)2P(NAg)(NHAg).(?)  SI.  sol.  in 
NH4OH+Aq.  (Stokes,  Am.  Ch.  J.  1894,  16. 
149.) 

Amidosulphonic  acid,  HOSO2NH2. 

Easily  sol.  in  H2O,  less  easily  in  alcohol. 
(Berglund,  B.  9.  252  and  1896.) 

Very  stable;  less  easily  sol.  in  H2O  than  its 
K  salt.  (Raschig,  A.  241.  177.) 

Stable  in  air.  Non-deliquescent  when  cold. 
Sol.  in  5  pts.  H2O  at  0°  and  in  2^  pts.  H2O 
at  70°.  Solution  in  H2O  can  be  boiled  several 
minutes  without  decomp.  Solubility  is  de- 
creased by  addition  of  H2SO4,  so  that  if 
1/5-1/4  pt.  H2SO4  is  added  to  H2O,  100  pts. 
of  the  liquid  dissolve  only  3  pts.  HOSO2NH2 
in  the  cold.  Pptd.  from  solution  by  HNO3 
or  glacial  acetic  acid,  but  not  by  HC1.  Solu- 
bility is  decreased  by  presence  of  NaHSO4. 
(Divers  and  Haga,  Chem.  Soc.  1896, 69. 1641.) 

Amidosulphonates. 

Easily  sol.  in  H2O;  si.  sol.  in  alcohol. 

Aluminum  amidosulphonate. 

Very  sol.  in  H20.  (Berglund,  Bull.  Soc. 
(2)  29.  422.) 

Ammonium  amidosulphonate,  (NH4)NH2SO3. 
Deliquescent.     Sol.  in  H2O;  insol.  in  al- 
cohol. 

Ammonium  silver  amidosulphonate, 

NH4S03(NH2),  AgS03(NH2). 
(Ephraim  &  Gurewitsch,  B.  1910,  43.  148.) 

Barium  amidosulphonate,  Ba(NH2SO3)2. 
Sol.  in  3  pts.  H2O.    (Berglund,  I.e.) 

Cadmium  amidosulphonate,  Cd(NH2SO3)2  + 

5H2O. 
Very  sol.  in  H2O.    (B.) 

Calcium    amidosulphonate,    Ca(NH2SO3)2  + 

4H20. 
Very  sol.  in  H2O.    (B.) 

Cobalt  amidosulphonate,  Co(NH2SO3)2  + 

3H2O. 
Sol.  in  H2O.    (B.) 

Copper    amidosulphonate,     Cu(NH2SO3)2 

2H2O. 
Sol.  in  H2O.    (B.) 

Gold     (auric)    potassium    amidosulphonate, 

K3Au2(NSO3)3. 
Very  si.  sol.  in  cold,  more  easily  sol.  in  hot 


H2O.     Sol.  in  dil.  HCl+Aq.     (Hofmann,  B. 
1912,  45.  1735.) 

Lead  amidosulphonate,  Pb(NH2S03)2+H20. 
The  most  sol.  of  all  amidosulphonates.  (B.) 

Lithium  amidosulphonate.    LiNH2SO3. 

Deliquescent.    (B.) 

Magnesium  amidosulphonate. 
Very  sol.  in  H2O. 

Manganese  amidosulphonate,  Mn(NH2SO3)2 

+3H2O. 
Very  sol.  in  H2O.    (B.) 

Mercuric  amidosulphonate.  basic, 
Hg(HgOS03NH2)2. 

Insol.  in  3.5  %  HNO3+Aq.  Very  sol.  in 
3  %  HCl+Aq.  (Hofmann,  B.  1912, 45. 1733. 

+2H2O.  Insol.  in  hot  H2O.  Sol.inKOH+ 
Aq.  (Divers  and  Haga,  Chem.  Soc.  1896,  69. 
1649.) 

Mercuric  potassium  amidosulphonate, 

KHgNS03. 

Very  si.  sol.  in  cold  H2O  and  cold  dil.  KOH 
+Aq.  Sol.  in  3  %  HCl+Aq.  (Hofmann,  B. 
1912,  46.  1732.) 

Mercuric   sodium   amidosulphonate, 

NaHgNSO3. 

Nearly  completely  sol.  in  hot  H2O.  (Hoff- 
mann, B.  1912,  45.  1734.) 

Nickel  amidosulphonate,  Ni(NH2SO8)2+ 

3H2O. 
Sol.  inH2O.    (B.) 

Potassium  amidosulphonate,  KNH2SO3. 
Sol.  inH2O.    (Berglund.) 

Potassium    silver   amidosulphonate, 

NHAgS03K+H2O. 

Decomp.  by  H2O;  sol.  in  NH4OH+Aq. 
(Hoffmann,  B"  1912,  45.  1734.) 

Silver  amidosulphonate,  AgNH2SO3. 
Sol.  in  15  pts.  H2O  at  19°  (B.) 

Sodium  amidosulphonate,  NaNH2S03. 
Sol.  in  H2O. 

Strontium  amidosulphonate,  Sr(NHoS03)2-f- 

4H2O. 
Sol.  in  H20. 

Thallium  amidosulphonate,  T1NH2SO3. 
Sol.  in  H20. 

Uranyl  amidosulphonate. 
Sol.  inH2O. 

Zinc  amidosulphonate,  Zn(NH2SO,)2+4H20. 
Sol.  in  H2O. 


16 


AMIDOSULPHUROUS  ACID 


Amidosulphurous  acid. 

Solubility  of  NH3  by  vol.  in  H2O  at  760  mm. 
and  t°:  1  vol.  H2O  at  760  mm.  and  t°  dis- 

Ammonium amidosulphite,  NH2  .  SO2  .  NH4. 

solves  V  vols.  NH3  gas,  vols.  reduced  to 

0°  and  760  mm 

Very  deliquescent.     Decomp.  in  the  air 
with  loss  of  NH3.    Sol.  in  H2O  with  decomp. 

ctllLl    1  \J\J  111111. 

t° 

v 

t° 

v 

Sol.  in  anhydrous  alcohol.     SI.  sol.  in  dry. 

ether.    (Divers,  Chem.  Soc.  1900,  77.  330.) 

0 

1049.60 

13 

759.55 

1 

1020.78 

14 

743.11 

Ammonia,  NH3. 

2 

993.26 

15 

727.22 

Very  sol.  in  H2O,  with  evolution  of  much 

3 

9S6.98 

16 

711.82 

.                  J 

heat. 

4 

941.88 

17 

696.85 

5 

917.90 

18 

682.26 

1  vol.  H2O  absorbs  670  vols.  (^  pt.  by  weight)  NHs 
at  +10°  and  29.8  in.  pressure;  sp.  gr.  of  solution  =0.875. 
(Davy.) 

6 

7 

894.99 
873.09 

19 
20 

667.99 
653.99 

At  low  temperatures  H2O  absorbs  more  than  %  its 

8 

852.14 

21 

640.19 

weight  of  NH3,  and  sp.  gr.  of  solution  =0.850.  (Dalton.) 
100  pts.  H2O  absorb  8.41  pts.  NHs  at  24°;  5.96  pts.  at 
55°.     (Osann.) 

9 
10 

831.98 
812.76 

22 
23 

626.54 
612.98 

1  vol.  HzO  absorbs  780  vols.  NHs,  6  vols.  H2O  in- 

11 

794.32 

24 

599.46 

creasing  to   10  vols.   sat.   NH4OH+Aq;   1   vol.   sat. 
NH4OH  +Aq  contains  468  vols.  NH3.    (Thomson.) 

12 

776.60 

25 

585.94 

1  vol.  H2O  absorbs  450  vols.  NHs  at  15°.     (Dumas.) 
1  vol.  H2O  absorbs  700  vols.  NHs  at  ordinary  temper- 

(Carius, A.  99.  144.) 

ature.    (Otto.) 

100  pts.  H2O  absorb  in  NHs  gas  47.7  pts.  NHs  by 

weight.    (Berzelius.) 
1  vol.  HzO  absorbs  505  vols.  NHs  and  vol.  is  in- 
creased to  1.5  vol.,  and  sp.  gr.  becomes  0.900.     (Ure.) 

Solubility  of  NH3  in  H20  at  P  mm.  pressure 
and  0°:  1  pt.  H2O  absorbs  pts.  NH3  at 

1  vol.  H20  at  0°  and  760  mm.  absorbs  1177.3 
vols.  NH3.  (Sims.) 

1  vol.  H20  at  0°  and  760  mm.  absorbs  1146 
vols.  NH3.  (Roscoe  and  Dittmar.) 

1  vol.  H2O  at  0°  and  760  mm.  absorbs 
1049.6  vols.  NH3.  (Carius.) 

1  vol.  H20  at  0°  and  760  mm.  absorbs  1270 
vols.  NH3.  (Berthelot.) 

1  vol.  H20  at  0°  and  760  mm.  absorbs  1050 
vols.  NH3.  (Bunsen.) 

100  cc.  H2O  absorb  64.50  g.  NH3. 
(Raoult.) 


Solubility  of  NH3  in  H2O  at  760  mm.  and  t°: 
1  g.  H20  absorbs  g.  NH3,  according  to 
Roscoe  and  Dittmar  (A.  122.  347)  (RD); 
and  according  to  Sims  (A.  118.  345)  (S). 


t° 

g.'NH, 
RD 

,NHs 

t° 

g.  NHs 
RD 

g.  NHs 

S 

0 

0.875 

0.899 

36 

0.343 

0  363 

2 

0  833 

0.853 

38 

0.324 

0.350 

4 

0.792 

0  809 

40 

0  307 

0.338 

6 

0.751 

0.765 

42 

0.290 

0  326 

8 

0  713 

0.724 

44 

0.275 

0.315 

10 

0.679 

0.684 

46 

0.259 

0.304 

12 

0.645 

0.646 

48 

0.244 

0.294 

14 

0.612 

0.611 

50 

0.229 

0.284 

16 

0.582 

0.578 

52 

0.214 

0.274 

18 

0.554 

0.546 

54 

0.200 

0.265 

20 

0.526 

0.518 

56 

0.186 

0.256 

22 

0  499 

0.490 

58 

0.247 

24 

0  474 

0.467 

60 

0  238 

26 

0^449 

0^446 

70 



0.194 

28 

0  426 

0  426 

80 

0.154 

30 

0^403 

0.408 

90 

0.114 

32 

0  382 

0.303 

98 

0.082 

34 

0.362 

0.378 

100 



0.074 

P  mm.  pressure  and  0°. 


P 

Pts.  NHs 

P 

Pts.  NH3 

10 

0.044 

900 

0.968 

20 

0.084 

950 

1.101 

30 

0.120 

1000 

1.037 

40 

0.149 

1050 

1.075 

50 

0.175 

1100 

1.117 

75 

0.228 

1150 

.161 

100 

0.275 

1200 

.208 

125 

0.315 

1250 

1.258 

150 

0.351 

1300 

1.310 

175 

0.382 

1350 

.361 

200 

0.411 

1400 

.415 

250 

0.465 

1450 

1.469 

300 

0.515 

1500 

1.526 

350 

0.561 

1550 

1.584 

400 

0.607 

1600 

1.645 

450 

0.646 

1650 

1.707 

500 

0.690 

1700 

1.770 

550 

0.731 

1750 

1.835 

600 

0.768 

1800 

1.906 

650 

0.804 

1850 

1.976 

700 

0.840 

1900 

2.046 

750 

0.872 

1950 

2.120 

800 

0.906 

2000 

2.195 

850 

0.937 

(Roscoe  and  Dittmar,  A.  112.  349.) 

In  proportion  as  the  temperature  is  higher, 
so  much  the  more  nearly  does  the  solubility  of 
NH3  in  H2O  conform  to  the  law  of  Henry  and 
Dalton,  but  only  obeys  it  completely  when 
the  temperature  is  100°,  as  is  seen  in  the  fol- 

lowing table. 

AMMONIA 


17 


Solubility  of  NH3  in  H2O  at  various  pressures  and  temperatures:  P  =  partial  pressure,  i.  e. 
total  pressure  minus  the  tension  of  aqueous  vapour  at  the  given  temperature;  G  =  grams 


NH3  dissolved  in  1  g.  H20  at  the  given  pressure;  G  at  760  =  grams  NH3  that  would 
be  contained  in  1  g.  H2O  if  the  solubility  was  proportional  to  the  pressure. 

P 

0° 

--—  —  —  -> 

G  at  P 

•*_———-— 
G  at  760 

20 

^•--   •«»  —  ~ 
Gat  P 

0 

-_-  —  •—  —  ^ 
G  at  760 

40 
G  at  P 

° 

-  -"*•  '  —-^ 
G  at  760 

100 

.  —  •  —  •  •*  —  ~- 
G  at  P 

• 

—  —  *-* 
Gat  760 

20 

0  082 

3   113 

30 

o!ii7 

2.960 



.... 

.... 

40 

0148 

2.820 

60 

.  J.^O 

0  169 

2  522 

0.119 

1  513 

\J\J 

80 

0.240 

2^280 

1^337 

0.052 

0.497 



100 

0  280 

2  127 

0  158 

1  200 

0.064 

0  490 

±\J\J 

120 

0^316 

2^000 

o!l73 

li095 

01076 

0.483 

140 

0.346 

1.880 

0.187 

1.017 

0.088 

0.476 

.... 

160 

0.375 

1.780 

0.202 

0.962 

0.099 

0.470 

.... 

180 

0.398 

1.684 

0.207 

0.918 

0.109 

0.462 



.... 

200 

0.421 

1.598 

0.232 

0.881 

0.120 

0.454 

.... 

250 

0.472 

.434 

0.266 

0.810 

0.145 

0.440 



.... 

300 

0.519 

.315 

0.296 

0.750 

0.168 

0.426 



.... 

350 

0.563 

.223 

0.325 

0.705 

0.191 

0.414 



.... 

400 

0.606 

.152 

0.353 

,0.670 

0.211 

0.402 



.... 

450 

0.650 

.100 

0.378 

0.638 

0.232 

0.399 



500 

0.692 

1.052 

0.403 

0.612 

0.251 

0.382 



.... 

550   ' 

0.732 

1.012 

0.425 

0.587 

0.269 

0.372 



.... 

600 

0.770 

0.975 

0.447 

0.566 

0.287 

0.363 

.... 

650 

0.809 

0.946 

0.470 

0.550 

0.304 

0.355 

.... 

700 

0.850 

0.923 

0.492 

0.534 

0.320 

0.347 

6!  068 

0.074 

750 

0.891 

0.903 

0.514 

0.521 

0.335 

0.339 

0.073 

0.074 

760 

0.899 

0.518 

0.518 

0.338 

0.338 

0.074 

0.074 

800 
850 
900 
950 
1000 
1050 
1100 
1150 
1200 
1250 
1300 
1350 
1400 

0^937 
0.980 
1.029 
1.077 
1.126 
1.177 
1.230 
1.283 
1.336 
1.338 
1.442 
1.496 
1.549 

0.888 
0.876 
0.869 
0.862 
0.855 
0.852 
0.850 
0.848 
0.846 
0.844 
0.843 
0.842 
0.841 

0.535 
0.556 
0.574 
0.594 
0.613 
0.632 
0.651 
0.669 
0.685 
0.704 
0.722 
0.741 
0.761 

0.504 
0.497 
0.485 
0.475 
0.466 
0.457 
0.450 
0.442 
0  433 
0.428 
0.422 
0.417 
0.413 

0.349 
0.363 
0.378 
0.391 
0.404 
0.414 
0.425 
0.434 
0.445 
0.454 
0.463 
0.472 
0.479 

0.332 
0.325 
0.319 
0.313 
0.307 
0.300 
0.294 
0.287 
0.282 
0.276 
0.271 
0.266 
0.260 

0.078 
0.083 
0.088 
0.092 
0.096 
0.101 
0.106 
0.110 
0.115 
0.120 
0.125 
0.130 
0.135 

0.074 
0.074 
0.074 
0.073 
0.073 
0.073 
0.073 
0.073 
0.073 
0.073 
0.073 
0.073 
0.073 

1450 

1.603 

0.840 

0.780 

0.409 

0.486 

0.255 





1500 

1.656 

0.839 

0.801 

0.406 

0.493 

0.250 





1600 

1.758 

0.835 

0.842 

0.400 

0.511 

0.242 





1700 

1.861 

0.832 

0.881 

0.394 

0.530 

0.237 



1800 

1.966 

0.830 

0.919 

0.388 

0.547 

0.231 



1900 

2.070 

0.828 

0.955 

0.382 

0.565 

0.226 

.... 

2000 

0  992 

0  377 

0  579 

0.220 



2100 

0.594 

0.215 





(Sims,  A.  118.  346.) 

18 


AMMONIA 


Solubility  of  NH3  in  H2O  at  temps,  below 
0°.     One  gram  H2O  dissolves 

Sp.  gr.  of  NH4OH+Aq,  according  to  lire  in 
Diet,  of  Arts. 

grams  NH3                 1  emp. 
0.947                    —3.9° 

%  NHs 

Sp.  gr. 

%NHs 

Sp.  gr. 

1  .  115                    —  10° 

1  768                    —  20° 

27.940 

0.8914 

15.900 

0.9363 

2  781                    30° 

27.633 

0.8937 

14.575 

0.9410 

2  946                    —  40° 

27.038 

0.8967 

13.250 

0.9455 

(Mallet,  Am.  Ch.  J.  1897,  19.  807. 
The  solubility  of  NH3  in  H2O  does  not 
follow  Dalton's  law  at  ord.  temp.,  but  does 
at  temp,  near  100°.     (Konowaloff,  J.  Russ. 
Phys.  Chem.  Soc.  1894,  26.   48;  Chem.  Soc. 
1896,  70  (2).  351. 

26.751 
26.500 
25.175 
23.850 
22.525 
21.200 
19.875 

0.8983 
0.9000 
0.9045 
0.9090 
0.9133 
0.9177 
0.9227 

11.925 
10.600 
9.275 
7.950 
6.625 
5.300 
3.975 

0.9510 
0.9564 
0.9614 
0.9662 
0.9716 
0.9768 
0.9828 

Sp.  gr.  of  NH4OH+  Aq. 

18.550 

0.9275 

2.650 

0.9887 

17.225 

0.9320 

1.325 

0.9945 

cr  TSJTT, 

^      * 

Sp.  gr.,  b.-pt.,  and  vols.  gas  in  NH4OH-f  Aq. 

32.3* 

OQ    or 

0.8750 

OOOK'T 

14.53 

1  Q    Aft 

0.9435 

26 
25.37* 

.ooO/ 

0.9000 
0.9054 

lo.^o 
12.40 
11.56 

0.9513 
0.9545 

%NH, 

Sp.  gr. 

B.-pt. 

Vols.  gas  in 
1  vol.  liquid 

22.07 
19.54 
17.52 

15.88 

0.9166 
0.9255 
0.9326 
0.9385 

10.82 
10.17 
9.6 
9.5* 

0.9573 
0.9597 
0.9616 
0.9632 

35. 
32. 

29. 

27. 

3 
6 
9 
3 

0.85 
0.86 
0.87 
0.88 

—3.3° 

+3.3° 
10° 
16.6° 

494 
456 
419 

382 

(H.  Davy,  Elements,  1.  241.) 

24. 

7 

0.89 

23.3° 

346 

*  By  direct  experiment.     The  other  numbers  were 
obtained  by  calculation,  making  no  allowance  for  com- 

22. 
19. 

2 

8 

0.90 
0.91 

30° 
36.6° 

311 

277 

pensation. 

17. 

4 

0.92 

43.3° 

244 

15 

I 

0  9 

9 

50° 

211 

Sp.  gr.  of  NH4OH+Aq  at  16°,  according  to 

12 

8 

0  94 

56  6° 

180 

Otto  in  his  Lehrbuch. 

10. 

5 

0.95 

63  3° 

147 

8. 

3 

0  S 

li 

70° 

116 

%  NHs 

Sp.  gr. 

%  NH3 

Sp.  gr. 

6 

2 

0.97 

78.3° 

87 

12.000 

0.9517 

8.500 

0.9650 

4. 

1 

0.98 

86.1° 

57 

11.875 

0.9521 

8.375 

0.9654 

2. 

0 

0.99 

91.1° 

28 

11.750 
11.625 

0.9526 
0.9531 

8.250 
8.125 

0.9659 
0.9664 

(Dalton,  in  New  System,  2 

.  422.) 

11.500 
11.375 

0.9536 
0.9540 

8.000 

7.875 

0.9669 
0.9673 

Sp.  gr.  of 

NH4OH+Aqsat 

.  at  t°. 

11.250 
11.125 

0.954i5 
0.9550 

7.750 
7.625 

0.9678 
0.9683 

t° 

Sp.  gr. 

t° 

Sp.  gr. 

t 

SP.  gr. 

11.000 
10.950 
10.875 
10.750 
10.625 
10.500 
10.375 
10.250 
10.125 

0.9555 
0.9536 
0.9559 
0.9564 
0.9569 
0.9574 
0.9578 
0.9583 
0.9588 

7.500 
7.375 
7.250 
7.125 
7.000 
6.875 
6.750 
6.625 
6.500 

0.9688 
0.9692 
0.9697 
0.9702 
0.9707 
0.9711 
0.9716 
0.9721 
0.9726 

0 
1 

2 

3 
4 
5 
6 

7 
8 

0.8535 
0.8561 
0.8587 
0.8611 
0.8635 
0.8658 
0.8681 
0.8703 
0  8725 

9 
10 
11 
12 
13 
14 
15 
16 
17 

0.8746 
0.8766 
0.8785 
0.8804 
0.8823 
0.8841 
0.8858 
0.8874 
0  8889 

18 
19 
20 
21 
22 
23 
24 
25 

0.8903 
0.8916 
0.8928 
0.8940 
0.8952 
0.8963 
0.8974 
0.8984 

10.000 

0.9593 

6.375 

0.9730 



9.875 

0.9597 

6.250 

0.9735 

(Carius, 

A.  99.  141.) 

9.750 

0.9602 

6.125 

0.9740 

• 

9.625 
9.500 
9.375 

0.9607 
0.9612 
0.9616 

6.000 
5.875 
5.750 

0,9745 
0.9749 
0.9754 

Sp.  gr.  of  NH4OH+Aq  at  14°, 
Carius  (A.  99.  148). 

according  to 

9.250 

0.9621 

5.625 

0.9759 

%  NHs 

Sp.    gr. 

%  NH3 

Sp.  gr 

9  125 

0  9626 

e     KAA 

OQ7fiA 

9.000 

0.9631 

5.375 

0.9768 

36.0 

0. 

8844 

35.2 

0  8860 

8.875 

0.9636 

5.250 

0.9773 

35.8 

0. 

8848 

35.0 

0  8864 

8.750 

0.9641 

5.125 

•0.9778 

35.6 

0. 

8852 

34.8 

0  8868 

8.625 

0.9645 

5.000 

0.9783 

35.4 

0. 

8856 

34.6 

0.8872 

AMMONIA 


19 


Sp.  gr.  of   NH4OH+Aq  at  14°,  etc;—  Cont. 

Sp.  gr.  of  NH4OH+Aq  at  14°,  etc.—  Cont. 

%  NHs 

Sp.  gr. 

%  NHS 

Sp.  gr. 

%  NHs 

Sp.  gr. 

%NH3 

Sp.  gr. 

34.4 

0.8877 

22.2 

0.9185 

10.0 

0.9593 

5.0 

0.9790 

34.2 

0.8881 

22.0 

0.9191 

9.8 

0.9601 

4.8 

0.9799 

34.0 

0.8885 

21.8 

0.9197 

9.6 

0.9608 

4  .  6 

0.9807 

33.8 

0.8889 

21.6 

0.9203 

9.4 

0.9616 

4.4 

0.9815 

33.6 

0.8894 

21.4 

0.9209 

9.2 

0.9623 

4.2 

0.9823 

33.4 

0.8898 

21.2 

0.9215 

9.0 

0.9631 

4.0 

0.9831 

33.2 

0.8903 

21.0 

0.9221 

8.8 

0.9639 

3.8 

0  .  9^839 

33.0 

0.8907 

20.8 

0.9227 

.  8.6 

0.9647 

.3.6  

0  9847 

32.8 

0.8911 

20.6 

0.9233 

8.4 

0.9654 

3.4 

0.9855 

32.6 

0.8916 

20.4 

0.9239 

8.2 

0.9662 

3.2 

0.9863- 

32.4 

0.8920 

20.2 

0.9245 

8.0 

0.9670 

3.0 

0.9873 

32.2 

0.8925 

20.0 

0.9251 

7.8 

0.9677 

2.8 

0.9882 

32.0 

0.8929 

19.8 

0.9257 

7.6 

0.9685 

2.6 

0.9890 

31.8 

0.8934 

19.6 

0.9264 

7.4 

0.9693 

2.4 

0.9899 

31.6 

0.8938 

19.4 

0.9271 

7.2 

0.9701 

2.2 

0.9907 

31.4 

0.8944 

19.2 

O.P277 

7.0 

0.9709 

2.0 

0.9915 

31.2 

0.8948 

19.0 

0.9283 

6.8 

0.9717 

1.8 

0.9924 

31.0 

0.8953 

18.8 

0.9289 

6.6 

0.9725 

1.6 

0.9932 

30.8 

0.8957 

18.6 

0.9296 

6.4 

0.9733 

1.4 

0.9941 

30.6 

0.8962 

18.4 

0.9302 

6.2 

0.9741 

1.2 

0.9950 

30.4 

0.8967 

18.2 

0.9308 

6.0 

0.9749 

1.0 

0.9959 

30.2 

0.8971 

18.0 

0.9314 

5.8 

0.9757 

0.8 

0.9967 

30.0 

0.8976 

17.8 

0.9321 

5.6 

0.9765 

0.6 

0.9975 

29.8 

0.8981 

17.6 

0.9327 

5.4 

0.9773 

0.4 

0.9983 

29.6 

OA      A 

0.8986 

OOQO1 

17.4 

1*7     O 

0.9333 

OAO  A  A 

5.2 

0.9781 

0.2 

0.9991 

29.4 
29.2 
29.0 

.  oyyl 
0.8996 
0.9001 

17.2 
17.0 
16  8 

.yo4u 
0.0347 
0  9353 

Hager  also  gives  a  table  in  his  Commentar 
zur  Pharmacopoea,  which  is  practically  iden- 

28.8 

0.9006 

16.6 

0.9360 

tical  with  those  here  given. 

28.6 

0.9011 

16.4 

0.9366 

28.4 
28.2 

0.9016 
0.9021 

16.2 
16.0 

0.9373 
0.9380 

Strength  of 

NH4OH+Aq  of  certain  sp.  gr. 
at  12°. 

28  0 

0  9026 

1  K    C 

0  9386 

,£O  .  w 

27.8 

0'9031 

J.U  .  O 

15.6 

0^9393 

—  — 

1  kg.  solu- 

1 1.   solu-     1  litre   consists  of 

27.6 

0.9036 

15.4 

0.9400            Sp.  gr. 

tion  con- 
tains e. 

tains  g.       H2O  in 

liquid   NHs 

27.4 

0.9041 

15.2 

-t  ~     f\ 

0.9407 

Of\  A  1  A 

NH8 

NH3            cc. 

in  cc. 

27.2 
27.0 

0  .  9047 
0.9051 

15.0 
14.8 

.9414 
0.9420 

0.870 

384.4 

334.5     535.5 

464.5 

26.8 

0.9057 

14.6 

0.9427 

0.880 

347.2 

305.5     574.5 

.425.5 

26.6 

0.9063 

14.4 

0.9434 

0.890 

311.6 

277.3     612.7 

387.3 

26.4 

0.9068 

14.2 

0.9441 

0.900 

277.3 

249.5     650.5 

349.5 

26.2 

0.9073 

14.0 

0.9449 

0.910 

244.9 

222.8     687.2 

312.8 

26.0 

0.9078 

13.8 

0.9456 

0  .  920 

213.4 

196.3      723.7 

276.3 

25.8 

0.9083 

13.6 

0.9463 

0.930 

182.9 

170.1      759.9 

240.1 

25.6 

0.9089 

13.4 

0.9470 

0.940 

152.9 

143.7     796.3 

203  7 

25.4 

0.9094 

13.2 

0.9477 

0.950 

124.2 

118.0     832.0 

168.0 

25.2 

0.9100 

13.0 

0.9484 

0  960 

97.0 

93.1      866.9 

133  .  1 

25.0 

0.9106 

12.8 

0.9491 

0.970 

70.2 

68.0     902.0 

98.0 

24.8 

0.9111   - 

12.6 

0.9498 

0.980 

45.3 

44.3     935.7 

64.3 

24.6 

0.9116 

12.4 

0.9505 

0.990 

21.0 

20.7     969.3 

30.7 

24.4 
24.2 

0.9122 
0.9127 

12.2 
12.0 

0.9512 
0.9520 

(Wachsmuth,  Arch.  Pharm;  (3) 

8.  510.) 

24.0 
23.8 
23.6 

0.9133 
0.9139 
0.9145 

11.8 
11.6 
11.4 

0.9527 
0.9534 
0:9542 

Sp.  gr.  of  NH4OH+Aqatl5°. 
(Most  careful  experiments.) 

23.4 
23.2 

0.9150 
0.9156 

11.2 
11.0 

0.9549 
0.9556 

Sp.  gr. 

%  NH3 

Sp.  gr. 

%NH3 

23.0 

22.8 
22.6 
22  4 

0.9162 
0.9168 
0.9174 
0.9180 

10.8 
10.6 
10.4 
10.2 

0.9563 
0.9571 
0.9578 
0.9586 

0.990 
0.974 
0.950 

2.15 
6.10 
13  54 

0.926 
0.916 
0.910 

19.50 
22:50 
24.40 

20 


AMMONIA 


Sp.  gr.  of  NH4OH+Aq  at  15°—  Continued 

Sp.  gr.  of  NH4OH+Aq  at  15°,  etc.—  Continued 

Sp.  gr.              %  NH3 

Sp.  gr. 

%  NH3 

Sp.  gr. 

%  NH3 

1  1.  contains 
g.  NH3 

Correction 
for*  1° 

0.900         27.70 
0.890         31.40 
0885         33.5 

0.882 
0.880 

34.8 
35.5 

0.966 
0.964 
0.962 
0.960 
0,958 
0.956 
0.954 
0.952 
0.950 
0.948 
0.946 
0.944 
0.942 
0.940 
0.938 
0.936 
0.934 
0.932 
0.930 
0.928 
0.926 
0.924 
0.922 
0.920 
0.918 
0.916 
0.914 
0.912 
0.910 
0.908 
0.906 
0.904 
0.902 
0.900 
0.898 
0.896 
0.894 
0.892 
0.890 
0.888 
0.886 
0.884 
0.882 

8.33 
8.84 
9.35 
9.91 
10.47 
11.03 
11.60 
12.17 
12.74 
13.31 
13.88 
14.46 
15.04 
15.63 
16.22 
16.82 
17.42 
18.03 
18.64 
19.25 
19.87 
20.49 
21.12 
21.75 
22.39 
23.03 
23.68 
24.33 
24.99 
25.65 
26.31 
26.98 
27.65 
28.33 
29.01 
29.69 
30.37 
31.05 
31.75 
32.50 
33.25 
34.10 
34.95 

80.5 
85.2 
89.9 
95.1 
100.3 
105.4 
110.7 
115.9 
121.0 
126.2 
*   131.3 
136.5 
141.7 
146.9 
152.1 
157.4 
162.7 
168.1 
173.4 
178.6 
184.2 
189.3 
194.7 
200.1 
205.6 
210.9 
216.3 
221.9 
227.4 
232.9 
238.3 
243.9 
249.4 
255.0 
260.5 
266.0 
271.5 
277.0 
282.6 
288.6 
294.6 
301.4 
308.3 

0.00026 
0.00027 
0.00028 
0.00029 
0.00030 
0.00031 
0.00032 
0.00033 
0.00034 
0.00035 
0.00036 
0.00037 
0.00038 
0.00039 
0.00040 
0.00041 
0.00041 
0.00042 
0.00042 
0.00043 
0.00044 
0.00045 
0.00046 
0.00047 
0.00048 
0.00049 
0.00050 
0.00051 
0.00052 
0.00053 
0.00054 
0.00055 
0.00056 
0.00057 
0.00058 
0.00059 
0.00060 
0.00060 
0.00061 
0.00062 
0.00063 
0.00064 
0.00065 

(Gruneberg,  Chem.  Ind.  12.  97.) 

The  following  table  is  calculated  from  the 
above  by  interpolation:  — 

Sp.  gr.            %  NHs 

Sp.  gr. 

%  NH3 

0.995           1  05 
0.990           2.15 
0.985           3.30 
0.980           4.50 
0.975           5.75 
0.970           7.05 
0.965           8.40 
0.960           9.80 
0.955         11  20 
0.950         12.60 
0.945         14.00 
0.940         15.45 

0.935 
0.930 
0.925 
0.920 
0  915 
0.910 
0.905 
0.900 
0.895 
0.890 
0.885 
0.880 

16.90 
18.35 
19.80 
21.30 
22  85 
24.40 
26.00 
27.70 
29.50 
31.40 
33.40 
35.50 

(Gruneberg.) 
Sp.  gr.  of  NH4OH+Aq  at  14°. 

%HN3 

Sp.  gr. 

%  NH3 

Sp.  gr. 

31 
23.8 
20  4 

0.8933 
0.9116 
0.9246 

15.6 
11.7 
5.1 

0.9400 
0.9536 
0.9780 

(Lunge  and  Smith,  B.  17.  777.) 

Sp.  gr.  of  NH4OH+Aq  at  15°,  according  to 
Lunge  and  Wiernik  (Zeit.  f.  angew.  Ch. 
1889.  183). 
(Most  carefully  worked  out  and  calculated.) 

Sp.  gr. 

%  NH3     1 

.  contains 
g.  NH3 

Correction 
for±  1° 

1.000 
0.998 
0.996 
0.994 
0.992 
0.990 
0.988 
0.986 
0.984 
0.982 
0.980 
0.978 
0.976 
0.974 
0.972 
0.970 
0.968 

0.00 
0.45 
0.91 
1.37 
1.84 
2.31 
2.80 
3.30 
3.80 
4.30 
4.80 
5.30 
5.80 
6.30 
6.80 
7.31 
7.82 

0.0 

4.5 
9.1 
13.6 
18.2 
22.9 
27.7 
32.5 
37.4 
42.2 
47.0 
51.8 
56.6 
61.4 
66.1 
70.9 
75.7 

0.00018 
0.00018 
0.00019 
0.00019 
0.00020 
0.00020 
0.00021 
0.00021 
0.00022 
0.00022 
0  00023 
0.00023 
0.00024 
0.00024 
0.00025 
0.00025 
0.00026 

NH3  is  much  less  sol.  in  KOH,  or  NaOH+ 
Aq  than  in  H2O. 

Solubility  of  NH3  in  H2O,  and  KOH-f-Aq 
of  various  strengths:  100  pts.  solvent 
absorbs  g.  NH3  at  t°. 

t°                H--0             KOH+Aq 
1                                   11.25%  KzO 

KOH+Aq 
25.25%  K2O 

0          90.00           72  00 
8          72.75       .    57.00 
16          59.75           46.00 
24          49.50           37.25 

49.50 
37.50 
28.50- 
21.75 

(Raoult,  A.  ch.  (5)  1.  262  } 

AMMONIA 


21 


100  pts.  sat.  KOH+Aq  dissolve  only  1  pt. 
NH3. 
Solubility  in  NaOH+Aq  is  the  same  as  in 
KOH+Aq  of  the  same  strength. 
NH4Cl+Aq  absorbs  slightly  less  NH3  than 
the  same  vol.  H2O.    NaNO3,  and  NH4NO3  + 
Aq  absorb  almost  the  same  amount  NH3  as 
the  same  vol.  H2O.    (Raoult,  I.e.) 

Solubility  of  NH3  in  100  pts.  Ca(NO3)2+Aq. 

Solubility  in  salts  +Aq  at  35°  C. 

Salt 

Concentration  of  the 
aq.  solution 

Mols.  NHj 
soluble  in  1  liter  of 
solution 

KC1 
NaCl 
CH3COOK 

H(COOK)2 
KOH 
NaOH 
HK2C03 
^Na2C08 

0  .  5  normal 

0.426  normal 
tt 

0.923    • 
0.966 
0.902 
0.902 
0.870 
0.896 
0.914 
0.932 

t° 

H20 

Ca(NO3)2+Aq 
28.38%Ca(NOi)i 

Ca(NO3)2+Aq 
59.03%Ca(NO3)2 

(Riesenfeld,  Z.  phys.  Ch.  1903,  45.  462.) 

The  solubility  of  NH3  in  NaNO3,  NH4NO3 
and  in  AgNO3,2NH3+Aq  is  nearly  the  same 
as  in  pure  H2O.    (Konowaloff,  C.  C.  1898,  II. 

659). 

0 

8 
16 

90.00 
72.75 
59.75 

96.25 
78.50 
65.00 

104.50 
84.75 
70.50 

(Raoult,  I.e.) 

Solubility  in  salt  solutions  at  25°C. 


Distribution-coefficient    of    NH3    between 
water  and  CHC13=26.3  at  20C;  24.9  at  25°; 
23.2  at  30°. 
The    distribution-coefficient    of    NH3    be- 
tween CHC13  and  a  number  of  salt  solutions 
has  been  determined  for  the  purpose  of  study- 
ing the  nature  of  metal-ammonia  compounds 
in  aqueous  solution.     (Dawson,  Chem.  Soc. 
1900,  77.  1242.) 

Distribution  of  NH3  between  H2O  and  CHC13 
at  18C. 

Salt 

Mols.  NHs  soluble  in 
1  liter  of 

5-normal 
solution 

1  -normal 
solution 

1.5-nor- 
mal 
solution 

KC1 
KBr 
KI 
KOH 
NaCl 
NaBr     ' 
Nal 
NaOH 
LiCl 
LiBr 
Lil 
LiOH 
KF 
KNO,      - 
KNOi 
KCN 
KCNS 
^K2S04 
^K2S03 
^K2C03 
^K2C204 
^K2Cr04 
CH.COOK 
HCOOK 
KB02 
KK2HPO4 
KNa2S 
KClO30.25-norm. 
KBrO30.25-norm. 
KI030.25-norm. 

0.930 
0.950 
0.970 
0.852 
0.938 
0.965 
0.995 
0.876 
0.980 
1.001 
1.030 
0.865 
0.839 
0.923 
0.920 
0.926 
0.932 
0.875 
0.865 
0.788 
0.866 
0.866 
0.866 
0.868 
0.814 
0.860 
0.887 
0.927 
0.940 
0.951 

0.866 
0.904 
0.942 
0.716 
0.889 
0.916 
0.992 
0.789 
1.008 
1.040 
1.094 
0.808 
0.722 
0.862 
0.855 
0.858 
0.868 
0.772 
0.768 
0.650 
0.771 
0.771 
0.765 
0.760 
0.677 
0.749 
0.795 

0.809 
0.857 
0.900 
0.607 
0.843 
0.890 
0.985 
0.716 
1  045 
1.090 
1.190 
0.768 
0.626 
0.804 
0.798 
0.802 
0.814 
0.678 
0.675 
0.554 
0.675 
0.675 
0.685 
0.678 
0.560 
0.664 
0.726 

NHs  concentration  in 
aqueous  solution, 
mo  Is.  /litre 

NHs  concentration  in 
CHCh  solution, 
mols./  litre 

0.9280 
1.921 
2.064 
2.274 
2.590 
3.700 
4.333 

0.03506 
0.07703 
0.08350 
0.09317 
0.1083 
0.1639 
0.1996 

(Dawson,  Z.  phys.  Ch.  1909,  69.  120.) 

Distribution  of  NH8  between  hydroxides  -f  Aq 
and  CHC13  at  18°. 

Aqueous  solution 

NHj  concen- 
tration in 
the  aqueous 
solution, 
mols.  /litre 

NHj  concen- 
tration in  the 
CHCls  solution, 
mols./litre. 

0.2-N.KOH 
0.5-N.  KOH 
0.2-N.  NaOH 
0.5-N.  NaOH 
0.2-N.  i^Ba(OH)2 
0.5-N.  KBa(OH)2 

1.949 
1.978 
2.016 
1.944 
2.076 
3.397 

0.0841 
0.0951 
0.0869 
0.0907 
0.08905 
0.1560 

(Abegg  &  Riesenfeld,  Z.  phys.  Ch.  1902,  40. 
100.) 

(Dawson,  I.e.} 

22 


AMMONIA 


Distribution  of  NH3  between  Cu(QH)2+Aq 
and  GHGls-at  18V     -- 

Solubility  of  NH3  in  ethyl  alcohol  (absolute) 
at  t°. 

Cone,  of  Cu(OH)2 
equivalents/  litre 

NHs   concentra- 
tion in  aqueous 
solution, 
mols./  litre 

NHs  concentra- 
tion in  CHCls 
solution, 
mols./litre 

t° 

%NH3 

Pts.  NHs  per  100  , 
pts.  alcohol 

0 
6 
11.7 
14.7 
17 
,  |    22 
L  .-28.4  ..... 

19.7 
17.1 
14.1 
13.2 
12.6 
10.9 
.1.  9.2 

24.5 
20.6 
16.4 
15,2 
14.7 
12.2 
10.1 

0.041 
0.0705 
0,081 

2.014 
2.653 
3.011 

0.07968 
0.1087 
0.1247 

Dawson,  I.e.) 

(r\o  Rrnvn    P     t     n    11.119.^ 

Sol.  in  3  pts.  alcohol  of  38°.     (Boullay.) 
1  vol.  alcohol  of  0.829  sp.  gr.  absorbs  about  50  vols. 
NHs.    (Davy.) 

Much  less  sol.  in  ethyl,  propyl,  or  amyl 
alcohol  than  in  H20.  (Pagliano  and  Emo, 
Gazz.  ch.  it.  13.  278.) 


1  vol.  abs.  alcohol  at  20°  and  760  mm. 
pressure  absorbs  340  vols.  NH3  gas.  (Miiller, 
W.  Ann.  1891,  43.  567.) 

1  1.  methyl  alcohol  sat  .-with  NHs  contains 
218  g.  NH3  at  0°;  sp.  gr.  of  solution  =  0.770 ; 
coefficient  of  solubility  =  425.0.  (Delepine) . 


Solubility  of  NH3  in  alcohol  at  t°:  weight  NH;3  =  weight  NH3  contained  in  a  litre  of  solution 
sat.  at  760  mm.  and  t°;  sp.  gr.  =  sp.  gr.;  of  solution;  C  =  coefficient  of  solubility . 


Temp. 

Degree  of  Alcohol 

100° 

90° 

80° 

70° 

60° 

50° 

0° 

Weight  NH3     . 

130.5 
0  782 

146.0 

0  783 

206.5 
0  808 

246.0 
0  830 

304.5 
0  835 

Q 

209.5 

245  (^ 

390  0 

504  5 

697  7 

10° 

Weight  NH3     . 
Sp.gr.     .     .     . 

108.5 
0.787 
164  3 

120.0 
0.803 
186  0 

167.0 
0.8DO 
288  0 

..... 

198.25 
0.831 
373  o 

227.0 
0.850 
438  6 

«r 

Weight  NH3     . 
gp.gr.     ...    ...... 

75.0 
0.791 
106  6 

97.5 

0.788 
147  8 

119.75 
0.821 
190  5 

137.5 
0.829 
223  0 

152.5 

0.842 
260  8 

•182.7 
0.869 

QQO    o 

30° 

Weight  NH3 
Sp.gr.     .     .     . 

51.5 
0.798 
97  0 

74.0 
0.791 

186  7 

81.75 
0.826 
121  6 

100.3 

129.5 
0.846 

Oil     A 

152.0 
0.883 

OKO    A 

(Detepine,  J.  Pharm.  (5)  25.  496.) 


Solubility  of  NH3  in  methyl  alcohol  (absolute) 
att°. 


t° 

%NHs 

Pts.  NHs  per  100 
pts.  alcohol 

0 
6 
11.7 
14.7 
17 
22 
28.4 

29.3 
26.0 
23.5 
21.8 
20.8 
18.3 
14.8 

41.5 
35.2 
30.7 
27.9 
26.3 
22.4 
17.4 

(de  Bruyn,  Z.c.) 

Readily  sol.  in  ether. 

Sol.  in,  0.4  vol.  petroleum  from  Amiano. 
(Saussure.) 

1  vol.  oil  of  turpentine  absorbs  7.5  vols. 
NH3  at  16°. 

1  vol..  oil  of  lemon  absorbs  8.5  vols.  NH3  at 
16°. 


1  vol.  oil  of  rosemary  absorbs  9.75  vols 
NH3  at  29°. 

1  vol.  oil  of  lavender  absorbs  47  vols.  NH3 
at  20°.  (Saussure.) 

1  vol.  caoutchine  absorbs  3  vols.  NH3 
(Himly.) 

Valerol  absorbs  much  NH3.  (Gerhardt,  A 
ch.  (3)  7.  278.) 

1  vol.  ether  at  760  mm.  pressure  absorbs 
17.13  vols.  NH3  at  0°;  12.35  vols.  at  10°  and 
10.27  vols.  at  15°.  (Christoff,  Z.  phys.  Ch. 
1912,  79.  459.) 

-f  H2O.    Colorless  crystals. 

+  KH2O.  Large  transparent  crystals 
(Rupert,  J.  Am.  Chem.  Soc.  1909,  31.  868.) 

Ammonia,  with  metal  salts. 

For  the  ammonia  addition-products  of 
metal  salts,  see  under  the  respective  metal 
salts,  except  in  the  case  of  Co,  Cr,  Hg,  and  the 
Pt  metals,  for  which  see  cobalt  ammonium, 
chromium  ammonium,  etc.,  compounds,  for 


AMMONIA 


23 


further  reference.  New  data  on  Co  and  Cr 
ammonium  compounds  and  those  of  the  Pt 
metals,  published  since  the  first  edition,  has 
not  been  included  in  the  present  edition. 

Ammonium  amalgam,  NH4,  a?Hg. 

Decomp.  by  H20,  but  more  easily  in  pres- 
ence of  naphtha,  alcohol,  or  ether. 

Ammonium  azoimide,  N4H4  =  NH4N3. 

Easily  sol.  in  H2O;  si.  sol.  in  absolute 
alcohol,  easily  in  80%  alcohol.  Insol.  in  ether 
or  benzene.  (Curtius,  B.  24.  3344.) 

Ammonium  cobalt  azoimide,  NH4N3,  CoN6. 

Rather  sol.  in  H2O.  (Curtius  and  Rissom, 
J.  pr.  1898,  (2)  68.  302.) 

Ammonium  bromide,  NH4Br. 


Sol.  in  liquid  NH3  at  —50°.  (Moissan 
C.  R.  1901,  133.  713.) 

Very  sol.  in  liquid  NH3.  (Franklin,  Am. 
Ch.  J.  1898,  20.  826.) 

SI.  sol.  in  alcohol. 

1  pt.  NH4Br  dissolves  in  32.3  pts.  alcohol 
(0.806  sp.  gr.)  at  15°;  9.5  pts.  at  78°.  (Eder, 
I.e.} 

100  pts.  absolute  methyl  alcohol  dissolve 
12.5  pts.  at  19°;  100  pts.  absolute  ethyl  al- 
cohol dissolve  3.22  pts.  at  19°.  (de  Bruyn, 
Z.  phys.  Ch.  10.  783.) 

Solubility  in  mixtures  of  methyl  and  ethyl 
alcohol  at  25°. 

P  =  %  methyl  alcohol  in  the  solvent. 
G  =  g.  NH4Br  in  10  cc.  of  the  solution. 
S  =sp.  gr.  of  the  sat.  solution  at  25°/4°. 


heat. 
1  pt.  NH4Br  dissolves  in  pts.  H20  at  t°. 

P 

G 

S 

0.00 
4.37 
10.40 
41.02 
80.69 
84.77 
91.25 
100.00 

0.255 
0.299 
0.321 
0.506 
0.813 
0.847 
0.934 
0.983 

0.8065 
0.8083 
0.8117 
0.8252 
0.8501 
0.8508 
0.8551 
0.8605 

t°      Pts.  H2O        t°       Pts.  H2O        t° 

Pts.  H2O 

10        1.51         30        1.23        100 
16        1.39        50        1.06 

0.78 

(Eder,  W.  A.  B.  82.  (2)  1284.) 

NH4Br+Aq  containing  41.09%  NH4Br  is 
sat.  at  15°.    (Gerlach.) 

Sp.  gr.  of  NH4Br+Aq  at  15°. 

(Herz,  Z.  anorg.  1908,  60.  156.) 

Solubility  in  mixtures  of  methyl  and  propyl 
alcohol  at  25°. 

P  =  %  propyl  alcohol  in  the  solvent. 
G  =  g.  NH4Br  in  10  cc.  of  the  solution. 
S  =  Sp.  gr.  of  the  sat.  solution  at  25°/4°. 

%  NH4Br 

Sp.  gr. 

%  NH4Br 

Sp.  gr. 

5 

10 
15 

1  .  0326 
1.0652 
1.0960 

20 
30 
41  09 

1.1285 
1.1921 
1.2920 

(Eder.) 
Sp.  gr.  of  NH4Br+Aq  at  16°. 

p 

G 

S 

0 
11.11 
23.8 
65.2 
91.8 
93.75 
100. 

0.983 
0.851 
0.690 
0.308 
0.128 
0.125 
0.095 

0.8605 
0.8524 
0.8426 
0.8184 
0.8097  , 
0.8089 
0.8059 

%  NEUBr 

Sp.  gr. 

%  NH4Br 

Sp.  gr. 

2 
3 
4 
5 
6 
.  7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
_'! 

1.0119 
1.0181 
1.0242 
1.0303 
1.0364 
1.0425 
1.0486 
1.0547 
1.0609 
1.0672 
1  .  0735 
1  .  0798 
1  .  0862 
1.0926 
1.0988 
1.1051 
1.1115 
1.1181 
1.1246 
1.1310 

22 
23 
24 
25 
26 
27 
28 
29 
'30 
31 
32 
33 
34 
35 
36 
37 
38 
39 
40 
41 

1.1375 
1.1440 
1.1506 
1.1573 
1.1642 
1.1713 
1.1787 
.1862 
.1938 
.2018 
.2098 
.2180 
.2260 
1.2342 
1.2425 
1.2509 
1  2594 
1.2679 
1.2765 
1.2850 

(Herz,  I.e.) 

Solubility  in  mixtures  of  propyl  and  ethyl 
alcohol  at  25°. 

P  =  %  propyl  alcohol  in  the  solvent. 
G  =  g.  NH4Br  in  10  cc.  of  the  solution. 
S  =Sp.  gr.  of  the  sat/  solution  at  25°/4°. 

P 

G 

S 

0 
8.1 
17.85 
56.6 
88.6 
91.2 
95.2 
100 

0.255 
0.251 
0.237 
0.163 
0.111 
0.105 
0.104 
0.095 

0.8065 
0.8062 
0.8052 
0.8048 
0.8042 
0.8049 
0.8059 
0.8059 

(Hager,  Comm.  1883.) 
25  g.  NH4Br+50  g.  H2O  lower  the  temp, 
from  15.1°  to  —1.1°.    (Rudorff.) 

(Herz,  I.e.) 

24 


AMMONIUM  BROMIDE 


Sol.  in  809  pts.  ether  (0.729  sp.  gr.)  .    (Eder, 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899. 
II,  1014);  (Naumann,  B.  1904,  37.  4328.) 

Insol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1370.) 

Insol.  in  methyl  acetate.     (Naumann,  B. 

1909,  42.  3790.) 

Insol.    in    ethylacetate.      (Naumann,    B. 

1910,  43.  314.) 

Ammonium  fnbromide,  NH4Br3. 

Gives  off  Br  in  air.  Sol.  in  H20.  (Rooze- 
boom,  B.  14.  2398.) 

Decomp.  in  the  air.  Very  sol.  in  H2O. 
(Chattaway,  Chem.  Soc.  1915,  107.  106.) 

Ammonium  antimony  bromide,  3NH4Br, 
2SbBr8. 

Easily  sol.  in  abs.  alcohol.  (Caven,  C.  C. 
1906.  II,  293.) 

7NH4Br,  3SbBrs.  Easily  sol.  in  abs.  al- 
cohol. (Caven,  C.  C.  1905.  II,  293.) 

See  also  Bromantimonate,  ammonium. 

Ammonium  bismuth  bromide.  NH4Br,  BiBr3 

+H20. 

Deliquescent.  Decomp.  by  H2O.  Sol.  in 
alcohol.  (Nickles,  C.  R.  61.  1097.) 

Ammonium  cadmium  bromide,  NH4Br, 


Sol.  in  0.73  pt.  H20,  5.3  pts.  abs.  alcohol, 
280  pts.  ether  (sp.  gr.  0.729),  and  24  pts. 
alcohol  ether  (1  :  1).  (Eder,  Dingl.  221.  89.) 

Sol.  in  H20  without  decomp.  between  1° 
and  110.1°. 
100  pts.  of  the  solution  contain  at: 

1°        14.8°    52.2°     110.1° 
53.82    58.01    65.32    75.83  pts.  of  the  salt. 

(Rimbach,  B.  1905,  38.  1555.) 

4NH4Br,  CdBr2.  Sol.  in  0.96  pt.  H20,  from 
which  it  is  pptd.  by  alcohol  or  ether.  (Eder.) 

Solubility  in  H2O  at  t°. 

Below  160°  the  salt  is  decomp.  by  H2O; 
at  160°  it  is  sol.  in  H2O  without  decomp. 


100  pts.  of  the 

solution  contain 

t° 

Solid  phase 

Pts. 

Pts. 

Pts. 

Cd 

Br 

NH4 

0.8 
13.0 

14.72 
14.94 

50.46 
51.48 

6.67 
6.85 

Double  salt+NH4Br 
(i 

44.5 

15.01 

53.85 

7.35 

(( 

76.4 

14.60 

55.28 

7.80 

<c 

123.5 

15.50 

59.50 

8.45 

It 

160.0 

14.70 

62.67 

9.43 

Double  salt 

(Rimbach,  B.  1905,  38.  1558.) 

Not  sol.  in  HBr+Aq  without  decomp. 
(Rimbach.) 

Not  sol.  without  decomp.  in  LiBr+Aq, 
CaBra+Aq,  MgBr2+Aq,  NiBr2-f-Aq,  or 


CoBr2+Aq,  even  though  very  cone,  solutions 
are  used.  Sol.  without  decomp.  in  ZnBr2+ 
Aq.  (Rimbach,  B.  1905,  38.  1571.) 

Ammonium     chloromolybdenum     bromide. 

2NH4Br,  Cl4Mo3Br2. 

Decomp.  by  pure  H2O.  Can  be  crystallized 
from  HBr+Aq.  Apparently  sol.  without 
decomp.  in  alcohol.  (Blomstrand.) 

Ammonium  cuprous  bromide. 

4NH4Br,  Cu2Br2.     Fairly  stable  in  air. 

2NH4Br,  Cu2Br2+H2O.  Fairly  stable  in 
air.  (Wells,  Z.  anorg.  1895,  10.  159.) 

Ammonium     cuprous     bromide     ammonia, 

NH4Br,  Cu2Br2,  3NH3. 
(Fleurent,  C.  R.  1891,  113.  1047.) 

Ammonium  cupric  bromide,  2NH4Br,  CuBr2 

+2H20. 
Very  sol.  in  H2O.     (de  Koninck,  B.  21. 

777  R.) 

Ammonium  indium  bromide. 
See  Bromiridate,  ammonium. 

Ammonium  iron  (ferric)  bromide, 

(NH4)FeBr4+2H2O. 

Very  deliquescent;  sol.  in  H2O.  (Walden, 
Z.  anorg.  1894,  7.  332.) 

Ammonium  lead  bromide,  12NH4Br.  7  PbBr2 
+7H20. 

Decomp.  on  air,  or  with  cold  H20.  (Andre, 
C.  R.  96.  1502.) 

6NH4Br,  PbBr2+H2O.  Decomp.  by  cold 
H20.  (A.) 

7NH4Br,  PbBr2  +  lHH2O.  Stable  on  air; 
decomp.  by  cold  H2O.  (A.) 

None  of  the  above  compounds  exist.  (Wells, 
Sill.  Am.  J.  146.  25.) 

2NH4Br,  PbBr2.  Decomp.  by  H2O.  Sol. 
in  cone.  KOH+Aq  and  in  strong  acids. 
(Fonzes-Diacon,  Bull.  Soc.  1897,  (3)  17.351.) 

NH4Br,  3PbBr2.    (Wells.) 

Ammonium    magnesium    bromide,    NH4Br. 

MgBr2+6H20. 

Deliquescent.  Sol.  in  H2O.  (Lerch,  J.  pr. 
(2)  28.  338.) 

Ammonium  mercuric  bromide, 

2HgBr2,  NH4Br. 

Decomp.  by  H20  into  its  constituent  salts. 
(Ray,  Chem.  Soc.  1902,  81.  648.) 

Ammonium  molybdenum  bromide,  2NH4Br, 

MoBr3+H2O. 

Easily  sol.  in  H2O.  (Rosenheim,  Z.  anorg. 
1905,  46.  322.) 

Ammonium  molybdenum  bromide  chloride. 

See  Ammonium  chloromolybdenum  bro- 
mide. 


AMMONIUM   CHLORIDE 


25 


Ammonium  osmium  bromide. 
See  Bromosmate,  ammonium. 

Ammonium  osmyl  bromide,  (NH4)2OsO2Br4 
Sol.  in  H2O.    (Wintrebert,  A.  ch.  1903,  (7 
28.  95.) 

Ammonium  osmyl  oxybromide, 

(NH4)2Os03Br2. 
(Wintrebert,  A.  ch.  1903.  (7)  28.  117.) 

Ammonium  palladium  bromide. 

See  Bromopalladate,  ammonium,  and 
Bromopalladite,  ammonium. 

Ammonium  platinum  bromide. 
See  Bromoplatinate,  ammonium. 

Ammonium  rhodium  bromide. 
See  Bromorhodite,  ammonium. 

Ammonium  selenium  bromide. 
See  Bromoselenate,  ammonium. 

Ammonium  tellurium  bromide. 
See  Bromotellurate,  ammonium. 

Ammonium  thallic  bromide,  NH4Br,  TlBr3  + 
2H20. 

Sol.  inH2O.    (Willm.) 

+4H2O.  Efflorescent.  Sol.  in  H2O 
(Nickles.) 

+5H2O.    Sol.  inH2O.    (Nickles.) 

Ammonium  stannous  bromide   (ammonium 

bromostannite),  NH4Br,  SnBr2+H2O. 
Sol.  in  H20.    (Benas,  C.  C.  1884.  958.) 
2NH4Br,  SnBr2.    Sol.  in  H2O.    (Raymann 

and  Preis,  A.  223.  323.) 

+H2O.    Sol.  in  H20.    (Benas,  I.e.) 
+2H2O.    (Richardson,  Am.  Ch.  J.  14.  96.) 
NH4Br,  2SnBr2(?).    (Benas.) 

Ammonium  stannic  bromide,  2NH4Br,  SnBr4. 
See  Bromostannate,  ammonium. 

Ammonium  uranyl  bromide,  2NH4Br,  UO2Br2 

+2H2O. 

Very  deliquescent,  and  sol.  in  H2O.  (Sendt- 
ner.) 

Ammonium  zinc  bromide,  2NH4Br,  ZnBr2. 

Deliquescent,  and  sol.  in  H2O.  (Bodeker, 
J.  B.  1860.  17.) 

+H2O.  Very  deliquescent,  and  sol.  in  H2O. 
(Andre",  A.  ch.  (6)  3.  104.) 

+zH2O.    (Ephraim,  Z.  anorg.  1908,  69. 66.) 

3NH4Br,  ZnBr2.  Sol.  in  H2O.  Decomp. 
only  by  great  dilution.  (Jones  &  Knight,  Am. 
Ch.  J.  1899,  22.  136.) 

+H2O.  Not  hygroscopic.  (Ephraim,  Z. 
anorg.  1908,  59.  66.) 

Ammonium  bromide  arsenic  in'oxide. 
See  Arsenite  bromide,  ammonium. 


Ammonium  bromide  mercuric  chloride, 

NH4Br,  2HgCl2. 
Ppt.    (Ray,  Chem.  Soc.  1902,  81.  649.) 

Ammonium  bromide  mercuric  iodide. 
2NH4Br,  HgI2. 

Decomp.  by  H2O.  Sol.  in  alcohol  without 
decomp.  (Grossmann,  B.  1903,  36.  1602.) 

3NH4Br,  2HgI2.  Decomp.  by  H2O.  Sol. 
in  alcohol  without  decomp.  (Grossmann,  B 
1903,  36.  1602.) 

Ammonium  lead  bromochloride, 
NH4Pb2Br4Cl. 

Decomp.  by  H2O.  (Fonzes-Diacon,  Bull. 
Soc.  1897,  (3)  17.  350.) 

NH4Pb2Cl4Br.  Decomp.  by  H2O.  (Fonzes- 
Diacon,  Bull.  Soc.  1897,  (3)  17.  349.) 

Ammonium  bromochloroiodide,  NH4ClBrI. 

Very  stable;  sol.  in  H2O.  (Chattaway, 
Chem.  Soc.  1915,  107.  108.) 

Ammonium -lead  bromoiodide,  NH4PbBrI2+ 

2H2O  and  NH4Pb2BrI4. 
Decomp.  by  H2O.    Sol.  in  cone.  KOH-f  Aq 
and  in  strong  acids.     (Fonzes-Diacon.  Bull. 
Soc.  1897,  (3)  17.  352.) 

Ammonium  bromiodobromide,  NH4BrIBr. 

Decomp.  in  the  air.  Sol.  in  ether.  (Jack- 
son, Am.  Ch.  J.  1900,  24.  28.) 

Ammonium  chloride,  NH4C1. 

(Sal-ammoniac.)  Not  deliquescent.  Sol. 
in  H2O  with  reduction  of  temp. 

Sol.  in  2.24  pts.  H2O.    (Wenzel.) 

NH4Cl+Aq  sat.  at  10°  has  sp.  gr.  =1.072.    (T.) 

Sol.  in  2.72  pts.  cold,  and  1  pt.  boiling  H2O.  (M.  R., 
and  P.) 

Sol.  in  3  pts.  HzO  at  18.75°.    (Abl.) 

Sol.  in  6  pts.  cold,  and  1  pt.  boiling  H2O.    (Fourcroy.) 

100  pts.  H2O  at  18.75°  dissolve  36.75  pts.  NH4C1. 

NH4CI+Aq  sat.  at  its  b.-pt.  (114.2°)  contains  88.9 
pts.  NHiCl  in  100  pts.  of  the  solution.  (Berzelius.) 

100  pts.  H2O  at  15°  dissolve  33-36  pts.;  and  at  100°, 
100  pts.  NH4C1.  (Ure's  Diet.) 

NH4Cl+Aq  sat.  at  15°  has  sp.  gr.  =1.075209,  and 
contains  at  least  31.88  pts.  NH4C1  dissolved  in  every 
100  pts.  H2O.  (Michel  and  Krafft,  A.  ch.  (3)  41.  478.) 

NH4Cl+Aq  sat.  at  10°  contains  23.8%  NH4C1. 
(Eller.) 

NH4C1  -f  Aq  sat.  in  the  cold  contains  14.3%  NH4C1. 
Fourcroy.) 

Sol.  in  1  pt.  H2O  at  113.5°,  b.-pt.  of  sat.  solution. 
Griffiths.) 

Sol.  in  2.7  pts.  H2O  at  18.75°,  forming  a  liquid  of  1.08 
p.  gr.  (Karsten,  1840.) 

Sol.  in  2.727  pts.  H2O  at  10°.    (Gren's  Handbuch.) 

00  pts.  H2O  at  718  mm.  pressure  and  t°  dissolve  pts. 


t° 

Pts. 
NH4C1 

t° 

Pts. 
NH4C1 

t° 

Pts. 
NH4C1 

t° 

Pts. 
NH4C1 

0 
10 
20 

28.40 
32.84 
37.28 

30 
40 
50 

41.72 
46.16 
50.60 

60 
70 
80 

55.04 
59.48 
63.92 

90 
100 
110 

68.36 
72.80 
77.24 

(Alluard,  C.  R.  89.  500  ) 

26 


AMMONIUM  CHLORIDE 


Solubility  in  100  pts.  H2O  at  t 


t° 

4 

t° 

4 

t° 

•  O 

2g 

t 

»q 

*§ 

0 

29.7 

30 

41.4 

60 

55.2 

90 

71.3 

1 

30.0 

31 

41.8 

61 

55.7 

91 

71.9 

2 

30.3 

32 

42:2 

62 

56.2 

92 

72.5 

3 

30.6 

33 

42.7 

63 

56.7 

93 

73.1 

4 

31.0 

34 

43.1 

64 

57.2 

94 

73.7 

5 

31.4 

35 

43.6 

65 

57.7 

95 

74.3 

6 

31.8 

36 

44.0 

66 

58.2 

96 

74.9 

7 

32.2 

37 

44.4 

67 

58.7 

97 

75.5 

8 

32.6 

38 

44.9 

68 

59.2 

98 

76.1 

9 

33.0 

39 

45.3 

69 

59.7 

99 

76.7 

10 

33.3 

40 

45.8 

70 

60.2 

100 

77.3 

11 

33.7 

41 

46.2 

71 

60.7 

101 

78.0 

12 

34.1 

42 

46.7 

72 

61.2 

102 

78.6 

13 

34.5 

43 

47.1 

73 

61.7 

103 

79.2 

14 

34.8 

44 

47.6 

74 

62.3 

104 

79.9 

15 

35.2 

45 

48.0 

75 

62.8 

105 

80.5 

16 

35.6 

46 

48.5 

76 

63.4 

106 

81.2 

17 

36.0 

47 

49.0 

77 

63.9 

107 

81.8 

18 

36.4 

48 

49.5 

78 

64.5 

108 

82.5 

19 

36.8 

49 

49.9 

79 

65.1 

109 

83.1 

20 

37.2 

50 

50.4 

80 

65.6 

110 

83.8 

21 

37.6 

51 

50.9 

81 

66.2 

111 

84.4 

22 

38.0 

52 

51.3 

82 

66.7 

112 

85.1 

23 

38.4 

53 

51.8 

83 

67.3 

113 

85.7 

24 

38.8 

54 

52.3 

84 

67.8 

114 

86.4 

25 

39.3 

55 

52.8 

85 

68.4 

115 

87.1 

26 

39.7 

56 

53.2 

86 

69.0 

115.65 

87.3 

27 

40.1 

57 

53.7 

87 

69.6 

28 

40.5 

58 

54.2 

88 

70.2 

29 

40.9 

59 

54.7 

89 

70.7 

(Mulder,  calculated  from  his  own  and  other 
observations.    Scheik.    Verhandel.  1864.  57.) 

Solubility  in  100  pts.  H2O  at  t°. 


t° 

Pts. 
NH4C1 

t° 

Pts. 
NH4C1 

t 

Pts. 
NH4C1 

0 

6.2 

29.7 
32.2 

10.8 
31.6 

33.9 
42.2 

64.9 
90.6 

57.9 
67.2 

(Lindstrom,  Pogg.  136.  315.) 

NH4Cl+Aq  sat.  at  13-16°  contains  26.16% 
NH4C1.  (v.  Hauer,  J.  pr.  103.  114.) 

Sol.  in  2.72  pts.  H2O  at  19°.  (Schiff,  A. 
109.  326.) 

Sol.  in  2.803  pts.  H2O  at  15°.    (Gerlach.) 

Sat.  NH4Cl+Aq  at  75°  contains  38.23% 
NH4C1.  (Tschugaeff,  Z.'anorg.  1914,  86. 161.) 

NH4Cl+Aq  sat.  at  30°  contains  29.5% 
NH4C1.  (Meerburg,  C.  C.  1904.  II,  1362.) 

Solubility  in  H2O  at  t°. 

1000  mols.  H2O  100  g.  H2O 

t°                  dissolve  dissolve 

mols.  NH4C1  g.  NH4C1 

3.5                 105.2  31.25 

25  0                 129.7  38.5 

50.0                 167.0  49.6 
(Biltz  and  Marcus,  Z.  anorg.  1911,  71. 169.) 


Solubility  of  NH4C1  in  H2O  at  t°. 


g.  NH4C1  in 

t° 

100  g.  of  the 

Solid  phase 

solution 

—  0.45 

0.78 

Ice 

—  1.25 

1.98 

i 

—  1.70 

2.76 

,~  •-         ( 

—  3.05 

4.6 

1 

—  4.45 

6.67 

t 

—  6.4 

.    9.23 

i 

—  8.25 

11.4 

t 

—  9.7 

13.1 

t 

—11.9 

15.3 

t 

—13.25 

16.7 

i 

—14.70 

18.  P 

i 

—15.4 

18.9 

t 

±—16.0 

±19.5 

Ice+NH4Cl 

—15.0 

19.7 

NH4C1 

—12.2 

20.0 

i 

—  10.9 

20.3 

i 

—  7.4 

21.1 

i 

—  5.7 

21.7 

i 

—  2.3 

22.3 

t 

±—  1.1 

22.6 

( 

0 

22.7 

it 

100  g.  H2O  dissolve  29.5  g.  NH4C1  at  30.° 
(Schreinemakers,  Arch.  neer.  Sc.  (2)  16.  17.) 

Spec,  gravity  of  NH4Cl+Aq.  G  =  according 
to  Gerlach  at  15°  (Z.  anal.  8.  281);  S  = 
according  to  Schiff  at  19°  (A.  110.  74). 


B 

Sp. 

gr. 

o 
H 

Sp. 

gr. 

S 

G 

S 

5 

G 

S 

1 

1.00316 

1.0029 

17 

1.05086 

1.0495 

2 

1.00632 

.0058 

18 

1.05367 

.0523 

3 

1.00948 

.0087 

19 

1.05648 

.0551 

4 

1  .  01264 

.0116 

20 

1.05929 

.0579 

5 

.  01580 

.0145 

21 

1.06204 

.0606 

6 

.01880 

.0174 

22 

1.06479 

.0633 

7 

.02180 

.0203 

23 

1.06754 

1.0660 

8 

.02481 

1.0233 

24  . 

1.07029 

1.0687 

9 

.02781 

1.0263 

25 

1.07304 

1.0714 

10 

.03081 

1.0293 

26 

1  .  07375 

1.0741 

11 

.  03370 

1  .  0322 

26.297 

1  .  07658 

12 

.03658 

1.0351 

27 

1  .  0768 

13 

1  .  03947 

1.0380 

28 

1  .  0794 

14 

1.04325 

1.0409 

29 

1.0802 

15 

1  .  04524 

1  .  0438 

30 

1.0846 

16 

1  .  04805 

1  .  Q467 

tor  older  determinations,  see  Storers  Diet. 
Sp.  gr.  of  NH4Cl+Aq  at  18°. 


%  NH4C1 

Sp.  [gr. 

%  NEUCl 

Sp.  gr. 

5 
10 
15 

1.0142 
1.0289 
1.0430 

20 
25 

1.0571 
1.0710 

(Kohlrausch,  W.  Ann.  1879.  1.) 


AMMONIUM  CHLORIDE 


27 


Sp.  gr.  at  20°/4°  of  a  normal  solution  of 
NH4C1  =  1.01454.  (Haigh,  J.  Am.  Chem. 
Soc.  1912,  34.  1151.) 

NH4Cl+Aq  containing  6.52%  NH4C1  has 
sp.  gr.  20720°  =  1.0195.  (Le  Blanc  &  Roh- 
land,  Z.  phys.  Ch.  1896,  19.  272.) 


Temp,  of  maximum 
density  of  NH<Cl+Aq 

g.  mol.  NH4C1  in 
1000  g.  H2O 

2.640° 
0.055° 

0.1899 
0.5407 

(de  Coppet,  C.  R.  1900,  131.  178.) 


Sp.  gr.  of  dil.  NH4Cl+Aq  at  20.004°  and  731 

mm.  (corr.) 
Cone.  =g.  equiv.  NH4C1  per  1.  at  20.004°. 


Cone. 

Sp.  gr. 

0.0000 

0.0001 
0.0002 
0.0005 
0.0010 
0.0020 
0.0050 
0.0100 

1.000,000,0 
1.000,001,8 
1.000,003,7 
1.000,009,3 
1.000,018,5 
1.000,036,9 
1.000,091,3 
1.000,180,3 

(Lamb  and  Lee,  J.  Am.  Chem.  Soc.  1913, 
35.  1688.) 

Sp.  gr.  of  dil.  NH4Cl+Aq. 


NHiCl  g.  in  1000  g. 
of  solution 

Sp.   gr. 
16°/16° 

0 
0.4431 
0.9061 
1.8085 
3.5947 
7.7845 
15.3425 
31.2364 

1.000000 
1.000150 
1  .  000304 
.  000606 
.001196 
.002562 
.  004994 
.  010018 

(Dijken,  Z.  phys.  Ch.  1897,  24.  107.) 


B.-pt.  of  NH4Cl+Aq,  containing  pts.  NH4C1 
to  100  pts.  H2O.  G  =  according  to  Ger- 
lach (Z.  anal.  26.  439);  L  =  according  to 
Legrand  (A.  ch.  (2)  59.  436). 


B.-pt. 

G 

L 

B.-pt. 

G 

L 

101° 

6.5 

7.8 

109° 

50.6 

53.5 

102 

12.8 

13.9 

110 

56.2 

59.9 

103 

19.0 

19.7 

111 

61.9 

66.4 

104 

24.7 

25.2 

112 

67.8 

73.3 

105 

29.7 

30.5 

113 

74.2 

80.5 

106 

34.6 

35.7 

114 

81.3 

88.1 

107 

39.6 

41.3 

114.2 

88.9 

108 

45.0 

47.3 

114.8 

87.1 

.... 

Sat,  NH4Cl-(-Aq  boils  at  115.8°  at  718  mm. 
pressure.  (Alluard,  C.  R.  59.  500.) 

NH4Cl+Aq  containing  74.2  pts.  NH4C1  to 
100  pts.  H2O  forms  a  crust  at  113°;  highest 
temperature  observed,  114.8°.  (Gerlach,  Z. 
anal.  26.  426.) 

NH4Cl+Aq  containing  10%  NH4C1  boils 
at  101.7°;  20%  NH4C1,  at  104.4°.  (Gerlach.) 

NH4Cl+Aq  containing  10.6%  NH4C1  gives 
off  NH3  at  37°.  (Leeds,  Am.  J.  Sci.  (3)  7. 
197.) 

When  NH4Cl+Aq  is  boiled,  or  even  evap. 
on  Water  bath,  a  little  NHs  is  expelled. 

(Fresenius.) 

30  pts.  NH4C1  mixed  with  100  pts.  H2O 
lower  the  temp,  from  13.3°  to  —5.1°,  that  is 
18.4°.  (Riidorff,  B.  2.  38.) 

Freezing-point  of  sat.  solution  is  — 15.4', 
the  same  temp,  which  is  caused  by  mixing  25 
pts.  NH4C1  with  100  pts.  snow.  (Rudorff, 
Pogg.  122.  337.) 

Cone.  HCl+Aq  precipitates  part  of  NH4C1 
from  sat.  NH4Cl+Aq.  (Vogel,  J.  pr.  2.  199.) 


Solubility  of  NH4C1  in  HCl+Aq  at  0°.  NH4C1 
=  mols.  NH4C1  (in  milligrammes)  dis- 
solved in  10  cc.  of  the  liquid;  HC1  = 
mols.  HC1  (in  milligrammes)  dissolved 'in 
10  cc.  of  the  liquid. 


NH4C1 

HCl 

Sum  of 
mols. 

Sp.  gr. 

46.125 

0.0 

46.125 

1.076 

43.6 

2.9 

46.5 

1.0695 

41.0 

5.5 

46.5 

1.0705 

39.15 

7.85 

47.0 

1.0715 

36.45 

10.85 

47.30 

1.073 

27.37 

21.4 

48.77 

1.078 

10.875 

53.0 

63.875 

1.106 

8.8 

61.0 

69.8 

1.114 

(Engel,  Bull.  Soc.  (2)  45.  655.) 


Solubility  of  NH4C1  in  HCl+Aq. 


t° 

HCl  concentra- 
tion, g.  mol.  per 
100  g.  H2O 

Weight   NH4C1 
dissolved    in 
1000  g.  H2O 

Molecular 
solubility 

0° 

0 

298.40 

5.59 

H 

286.43 

5.36 

Y2 

271.23 

5.08 

1 

245.35 

4.60 

25° 

0 

395.10 

7.40 

1A 

380.85 

7.13 

% 

366.00 

6.85 

339.05 

6.35 

(Armstrong  &  Eyre,  Proc.  R.  Soc.  (A.)  84. 
127.) 


28 


AMMONIUM  CHLORIDE 


Solubility  in  NH4OH+Aq.  NH4Cl  =  mols. 
NH4C1  (in  mgs.)  in  10  cc.  solution; 
NH3  =  mols.  NH3  (in  mgs.)  in  10  cc. 
solution. 


NHiCl 

NHj 

Sp.  gr. 

46.125 

0 

.076 

45.8 

5.37 

.067 

45.5 

12.025 

.054 

45.125 

23.4 

.044 

44.5 

38.0 

.031 

44.0 

47 

.025 

43.625 

54.5 

.017 

43.125 

80.0 

0.993 

44.0 

90.0 

0.992 

44.375 

95.5 

0.983 

49.75 

130 

0.953 

60.0 

169.75 

0.931 

(Engel,  Bull.  Soc.  (3)  6.  17.) 

NH4Cl+BaCl2.  100  pts.  H20  dissolve  33.8 
pts.  NH4C1+11.6  pts.  BaCl2  at  20°.  (Rudorff, 
Pogg.  148.  467.) 

Solubility  of  NH4C1  and  BaCl2  in  H20. 


Wt.  per  100 


NH4C1 


16.10 

19.26 
24.89 
26.93 
29.53 


BaCU 


8.07 
8.22 
8.19 
8.40 
8.55 


Solid  phase 


NH4C1+ 
BaCl2.2H2O 


(Schreinemakers,Chem.  Weekbl.  1910, 7. 333.) 
See  also  BaCl2+NH4Cl  under  BaCl2. 

NH4Cl+CdCl2.    Solubility  of  NH4C1  and 
CdCl2. 
See  Ammonium  cadmium  chloride. 

NH4Cl+CuCl2.  Solubility  of  NH4C1  in 
H2O  at  30°  in  presence  of  varying  amounts  of 
CuCl2. 


%by 

wt. 

CuCU 


0 

1.9 
3.6 
7.7 
10.5 
12.3 
15.6 
19.9 
24.0 
29.4 
35.1 
41.4 
43.2 
43.9 


%by 

wt. 
NH4C1 


29.5 
28.6 
25.9 
•19.8 


16.5 

14.9 

12.1 

9.4 

7.1 

4.9 

3.4 

2.1 

2.0 

0. 


Solid  phase 


NHiCl 

NHiCl+CuClz,  2NH4C1.  2H2O 
CuCl2,  2NH4C1.  2H2O 


CuCIa,  2NH«C1.  2H2O  +CuCU.  2H20 
CuCh.  2HsO 


NH4Cl+PbCl2.     Solubility  of  NH4C1  and 
PbCl2  in  H2O  at  22°. 


g.  equivalent 
in  1000  g.  H2O 


NH4C1 


0.0 
0.1 
0.2 

0.3 

0.4 

0.5 

0.52 

0.55 

0.6 

0.65 

0.7 

0.8 

0.9 

1.0 

1.2 

1.5 

2.0 

2.5 

3.0 

4.0 

5.0 

6.0 

7.0 

7.29 

7.29 


PbCh 


0.0749 
0.0325 
0.0194 
0.0153 
0.0138 
0.0130 
0.0127 
0.0123 
0.0113 
0.0105 
0.0099 
0.0087 
0.0083 
0.0080 
0.0075 
0.0073 
0.0077 
0.0092 
0.0112 
0.0182 
0.0296 
0.0473 
0.0774 
0.0898 
0.0000 


Solid  phase 


PbCl2 


PbCl2+NH4Cl,2PbCl2 
NH4C1, 2PbCl2 


NH4Cl+NH4Cl,2PbCl2 
NH4C1 


(Bronstedt,  Z.  phys.  Ch.  1911,  77.  132.) 


Solubility  of  NH4C1  and  2PbCl2,NH4Cl  in 
H2O  at  100°. 


NH4C1 
g.  equivalent 

PbCh 
g.  equivalent 

Solid  phase 

o§ 

31 

bC 

§o 

SK 

a 

*d 
§1 

S.3 

.SS 

ti 

s° 

2M 
a 

1.277 

1.404 

0.160 

0.176 

NH4C1 
+2PbCl2.H20 

(Bronstedt,  I.  c.) 


NH4Cl+MgCl2.     Solubility  of  NH4C1  and 
NH4MgCl3.6H20. 


3.5° 
25 
50 


In  1000 
mols.    H 


F;     .a  .s 


27.5 
42.1 
62.9 


55.7 
56.4 
59.1 


Solid  phase 


NH4Cl+NH4MgCl3 .6H2O 


(Meerburg,  Z.  anorg.  1905,  46.  3) 


(Biltz  and  Marcus,  Z.  anorg.  1911,  71.  170.) 


AMMONIUM  CHLORIDE 


29 


Solubility  of  NH4MgCl3.6H2O  and  MgCl2 
6H20. 


3.5° 
25° 
50° 


In  1000  g.  mol.  H2O 


mol. 


g.  mol. 
NH4C1 


0.5 

0.5 

0.8 


g.  mol. 
MgCls 


99.5 

103.8 
111.2 


Solid  phase 


MgCl2.  6H2O  + 
NH4MgCl3.6H20 


(Biltz  and  Marcus,  Z.  anorg.  1911,  71.  170.) 


NH4C1+NH4NO3.     100  pts.  H2O  dissolve 
.lpts.NH4Cl+17< 
(Riidorff,  B.  6.  482.) 


29.1  pts.  NH4C1+173.8  pts.  NH4NO3  at  19.5°. 
,iidc 


NH4Cl+Ba(NO3)2.    100  pts.  H2O  dissolve 
at  18.5°— 


1 

2 

3 

4 

5 

NH4C1 

Ba(NO,)s 

36.7 

38.6 
8.6 

38.06 
16.73 

39.18 
17.02 

S.9 

2,  sat.  Ba(NO3)2+Aq  treated  with  NH4C1; 

3,  sat.  NH4Cl+Aq  treated  with  Ba(NO3)2; 

4,  simultaneous  treatment  of  both  salts  with 
H2O.    (Karsten.) 

NH4C1+KNO3.     100  pts.  H2O  dissolve  at 
18.5°— 


1 

2 

3 

4 

5 
36'7 

6 

KNO3 
NH4C1 

29.9 

30.56 
44.33 

37.68 
37.98 

38.62 
39.84 

34.2 

38.8 

74.89 

75.66 

78.46 

73.0 

1  and  5,  according  to  Mulder;  2,  sat.  KNO3 
+Aq  treated  with  NH4C1;  3,  sat.  NH4Cl+Aq 
treated  with  KNO3;  4,  simultaneous  treat- 
ment of  NH4C1  and  KNO3  (Karsten) ;  6,  by 
warming  solution  with  excess  of  both  salts. 
and  cooling  to  14.8°.  The  amount  of  excess 
of  one  or  the  other  salt  has  no  influence. 
(Rudorff.) 

NH4Cl+NaNO3.  Slowly  sol.  in  sat. 
NaNO3-(-Aq,  at  first  to  a  clear  solution,  but 
afterwards  NaCl  separates  out.  (Karsten.) 

NH4C1+KC1.    100  pts.  H2O  dissolve— 


KC1 
,NH4C1     . 

(Rudorff) 
15° 

(Karsten) 
18.75° 

16.97 
28.90 

34.4 

16.27 
29.83 

37^02 

KC1     .     . 
NH4C1     . 

(Rudorff) 
22° 

(Mulder) 
At  b.-pt. 

19.1 

30.4 

58.5 

21.9 
67.7 

87'3 

100  pts.  sat.  solution  of  NH4C1+KC1  con- 
tain 30.61  pts.  of  the  two  salts  at  13-16°.  (v. 
Hauer,  J.  pr.  103.  114.) 


NH4Cl+NaCl.    100  pts.  H2O  dissolve 


NH4C1  . 

NaCl.     . 

(Mulder) 
10-20°          10°            10° 

(v.  Hauer) 
13-16° 

35.8 

19.50 
30.00 

33.3 

18.8-20.3 
24.6-26.1 

49.50 

43.4-46.4 

NH4C1 
NaCl 

(Karsten) 
18.75° 

(Rudorff) 
18.7° 

(Mulder) 
At  b.-pt. 

22.06 
26.38 

48.44 

37.02 

22.9 
23.9 

87.3 

78.5 
22.3 

40]i 

46.8 

100.8 

Sp.  gr.  of  sat.  solution  of  NH4Cl+NaCl  is 
1.179.  (Karsten.) 

NH4C1+(NH4)2SO4.  100  pts.  H2O  dis- 
solve 26.8  pts.  NH4Cl+46.5  pts.  (NH4)2SO4 
at  21.5°.  (Rudorff,  B.  6.  484.) 

Solubility  in  (NH4)2SO4+Aq  at  30°. 


Composition  of  the 
solution 


%  by  wt. 
NH4C1 


0 

6.86 
14.62 
17.60 
17.93 
19.07 
19.97 
22.3 
24.06 
29.5 


%  by.  wt. 
(NH4)2S04 


44 

36.15 
28.6 
25.69 
25.81 
23.22 
21.3 
16.33 
12.72 
0 


Solid  phase 


(NH4)2S04 
u 

t( 

(NH4)2S04+NH4C1 

u 

NH4C1 


(Schreinemakers,  Z.  phys.  Ch.  1909,  69.  562.) 

NH4Cl+CuSO4.  Sol.  in  sat.  CuSO4+Aq, 
at  first  to  a  clear  solution,  but  a  double  sul- 
phate of  NH4  and  Cu  soon  separates.  (Kar- 
sten.) 

NH4Cl+MgSO4.  Slowly  and  difficultly  sol. 
in  sat.  MgSO4+Aq  with  subsequent  separa- 
tion of  double  sulphate.  (Karsten.) 

NH4C1+K2SO4.  100  pts.  H20  dissolve,  at 
18.75°— 


K2S04 
NH4C1 


10.8 


11.1 
38.2 


13.26 
37.94 


49.3    51.20 


13.28 
37.92 


51.20 


36.7 


In  (a)  NH4C1  was  added  to  sat.  K2SO4+Aq. 
In  (6)  K2SO4  was  added  to  sat.  NH4Cl+Aq. 
In  (c)  NH4C1  and  K2SO4  were  treated  to- 
gether with  H2O.    (Karsten.) 


30 


AMMONIUM  CHLORIDE 


100  pts.  H2O  at  14°  dissolve  14.1  pts 
K2SO4+36.8  pts.  NH4C1  =  50.9  pts.  K2SO4+ 
NH4C1,  under  all  conditions.  (Riidorff,  Pogg 
148.  565.) 

100  pts.  H2O  dissolve  at  b.-pt. — 


K2SO4  . 
NH4C1 . 


26.75 


33.3-  33.9 
90.4-111.8 


123.7-145.7 


87.3 


(Mulder.) 

NH4Cl+Xa2SO4.  100  pts.  H2O  dissolve 
28.9  pts.  XH4Cl+24.7  pts.  Na2SO4,  if  NH4C1 
+Aq  sat.  at  10°  is  sat.  with  Na2SO4  at  11°. 

100  pts.  H2O  dissolve  31.8  pts.  NH4Cl-f- 
9.0  pts.  Na2SO4,  if  Na2SO4+Aq  sat.  at  10°  is 
sat.  with  NH4C1  at  11°.  (Mulder,  J.  B.  1866 
68.) 

Sol.  in  sat.  Na2S04+Aq.    (Karsten.) 

Sol.  in  sat.  ZnSO4+Aq.    (Karsten.) 

SI.  sol.  in  liquid  NH3  at  —50°.  (Moissan, 
C.  R.  1901,  133.  713.) 

Very  sol.  in  liquid  NH8.  (Franklin,  Am. 
Ch.  J.  1898,  20.  826.) 

Very  si.  sol.  in  absolute  alcohol. 

100  pts.  alcohol  of  0.939  sp.  gr.  dissolve— 

at  4°    8°       27°     38°    56° 

11.2   12.6   19.4  23.6   30.1   pts.   NH4C1. 
(Gerardin,  A.  ch.  (4)  5.  129.) 

14  pts.  boiling  highest  rectified  spirit  dissolve  1  pt. 
NEUCL    (Wenzel.) 
100  pts.  alcohol  of— 

0.900  sp.  gr.  dissolve  6.5    pts.  NH4C1. 
0.872    "     "         "        4.75    " 
0.834    "     "         "        1.5       " 
(Kinvan.) 

Though  somewhat  sol.  in  pure  absolute 
alcohol,  NH4C1  is  absolutely  insol.  in  alcohol 
in  presence  of  methyl  amine  chlorides. 
(Winkles,  A.  93.  324.) 

100  pts.  absolute  methyl  alcohol  dissolve 
3.35  pts.  at  19°. 

100  pts.  absolute  ethyl  alcohol  dissolve  0.62 
pt.  at  19°.  (de  Bruyn,  Z.  phys.  Ch.  10.  783.) 

Solubility  of  NH4C1  in  methyl  alcohol. 


Alcohol  concen- 

> 

tration,  mol.  g. 
alcohol    for 
1000  g.  H2O 

Solubility 
in  1000  g.  H2O 

Molecular 
solubility 

0° 

0 

298.40 

5.59 

u 

% 

297.35 

5.57 

(I 

1A 

296.55 

5.55 

11 

i 

292.65 

5.47 

(( 

3 

283  .  15 

5.30 

25° 

0 

395.10 

7.40 

« 

y* 

394.75 

7.39 

(i 

& 

393  85 

7  37 

a 

i 

392.90 

7.36 

•  (c 

3 

386.20 

7.23 

(Armstrong  and  Eyre,  Proc.  R.  Soc.  Lond.  (A) 
84.  127.) 


Alcohol  concen- 

t° 

tration,   mol.  g. 
alcohol  for 
1000  g.  H2O 

Solubility  in 
1000  g.  H2O 

Molecular 
solubility 

0° 

0 

298.46 

5.59 

( 

M 

295.40 

5.53 

I 

M 

291.30 

5.45 

{ 

1 

284.00 

5.32 

25° 

0 

395.10 

7.40 

< 

H 

393.50 

7.37 

' 

1A 

390.80 

7.32 

i 

i 

384.80 

7.21 

Solubility  of  NH4C1  in  ethyl  alcohol  at  0°. 


Alcohol   concentration, 
mol.  g.  alcohol  for 
1000  g.  H2O 

Solubility  in 
1000  g.  H2O 

Molecular 
solubility 

0 

298.40 

5.59 

M 

295.50 

5.53 

/^ 

291.95 

5.47 

i 

286.40 

5.37 

3 

266.25 

4.99 

(Armstrong  and  Eyre,  I.e.) 
See  also  ammonium  cupric  chloride. 
Solubility  of  NH4C1  in  propyl  alcohol. 


(Armstrong  and  Eyre,  I.e.) 

Solubility  in  mixtures  of  methyl  and  ethyl 

alcohol  at  25°. 

P  =  %  methyl  alcohol  in  the  solvent. 
G  =  g.  NH4C1  in  10  cc.  of  the  solution. 
S  =  sp.  gr.  of  the  sat.  solution  at  25°/4°. 


P 

G 

s 

0.00 
4.37 
10.40 
41.02 
80.69 
84.77 
91.25 
100.00 

0.0533 
0.0583 
0.0658 
0.118 
0.217 
0.227 
0.247 
0.276 

0.7908 
0.7909 
0.7910 
0.7957 
0.8020 
0.8026 
0.8040 
0.8062 

(Herz,  Z.  anorg.  1908,  60.  155.) 

Solubility  in  mixtures  of  methyl  and  propyl 
alcohol  at  25°. 
P  =  %  propyl  alcohol  in  the  solvent. 
G  =  g.  NH4C1  in  10  cc.  of  the  solution. 
S  =  Sp.  gr.  of  the  sat.  solution  at  25°/4°. 

p 

G 

S 

0 
11.11 
23.8 
65.2 
91.8 
93.75 
100.00 

0.276 
0.231 
0.182 
0.071 
0.026 
0.023 
0.018 

0.&062 
O.S035 
0.8008 
0.8005 
0.8002 
Or8000 
0.8009(?) 

(Herz,  Z.  anorg.  1908,  60.  157.) 

AMMONIUM  CADMIUM  CHLORIDE 


31 


Solubility  in  mixtures  of  propyl  and  ethyl 

alcohol  at  25°. 

p  =  %  propyl  alcohol  in  the  solvent. 
G  =  g.  NH4C1  in  10  cc.  of  the  solution. 
S  =  Sp.  gr.  of  the  sat,  solution  at  25°/4°. 


p 

G 

s 

0 

0.0533 

0.7908 

8.1 

0.0505 

0.7910 

17.85 

0.0455 

0.7916   ' 

56.6 

0.0312 

0.7963 

88.6 

0.0210 

0.7996 

91.2 

0.0203 

0.8001 

95.2 

0.0190 

0.8003  . 

100 

0.0177 

0.8009 

(Herz,  Z.  anorg.  1908,  60.  160.) 

Insol.  in  ether  and  CS2.  (Fordos  and  Gelis, 
A.  ch.  (3)  32.  393.) 

Very  si.  sol.  in  acetone.  (Krug  and  M'El- 
roy,  J.  anal.  appl.  Ch.  6.  184.) 

Solubility  of  NH4C1  in  acetone +Aq  at  25°. 
I  A  =  cc.  acetone  in  100  cc.  acetone +Aq. 
;-   NH4C1  =millimols.  NH4C1  in  100  cc.  of  the 
solution. 


A 

NH4C1 

Sp.  gr. 

0 

585.1 

1  .  0793 

10 

534.1 

1.0618 

20 

464.6 

1.0451 

30 

396.7 

1  .  0263 

40 

328.5 

0.99984 

46.5) 

lower 

283.7 

0.97998 

to       2 

phases 

85.  7J 

upper 

18.9 

0.8390 

90 

9.4 

0.8274 

(Herz,  Z.  anorg.  1905,  46.  263.) 
Solubility  of  NH4C1  in  glycerine +Aq  at  25° 
G  =  g.  glycerine  in  100  g.  glycerine +Aq. 
NH4Cl  =  millimols.  NH4C1  in  100  cc.  of  th 
solution. 


G 


0 

13.28 
25.98 
45.36 
54.23 
83.84 
100 


NHiCl 


585.1 
544.6 
502.9 
434.4 
403.5 
291.4 
228.4 


Sp.  gr. 


.0793 
.0947 
.1127 
.1452 
.1606 
.2225 
1.2617 


(Herz,  I.e.) 

Insol.  in  acetone.    (Naumann,  B.  1904,  37 
4328.);  (Eidmann,  C.  C.  1899.  II,  1014.) 

Insol.  in  anhydrous  pyridine.    Sol.  in  97 °/ 
pyridine+Aq,  95%  pyridine +Aq  and  in  93  < 
pyridine+Aq.     (Kahlenberg,  J.  Am.  Chem 
Soc.  1908,  30.  1107.) 

Insol.  in  CS2.     (Arctowski,  Z.  anorg.  1894 
6.  257.) 

Very  sol.  in  ethyl  amine.     (Shinn,  J.  phys 
Chem.  1907,  11.  538.) 

Insol.  in  methyl  acetate.     (Xaumann,  B 
1909,  42.  3790.) 


Insol.  in  ethyl  acetate.  (Naumann,  B» 
910,  43.  314.) 

Insol.  in  benzonitrile.  (Naumann,  B.  1914, 
7.  1370.) 

Sol.  in  formic  acid.  (Zanninovich-Tessarin, 
.  phys.  Ch.  1896,  19.  251.) 

Ammonium  antimony  chloride,  SbCl6(NH4)2, 
SbCl6(NH4)3. 

Ppt.  Decomp.  by  H2O.  (Weinland,  B. 
905,  38.  1085.) 

SbCl6(NH4),SbCl6,NH4OH.  Very  deli- 
mescent;  si.  sol.  in  H2O  with  decomp.  (Wein- 
and,  B.  1901,  34.  2635.) 

Ammonium    antimonous    chloride,    NH4C1, 

SbCl3. 

Deliquescent.    (Deherain,  C.  R.  52.  734.) 
2NH4C1,  SbCl3+2H2O.    Permanent  in  dry 

lir;  decomp.  by  much  H2O.    (Poggiale.) 
3NH4C1,  SbCl3+3H2O.    As  above. 

Ammonium  antimonic  chloride,  3NH4C1, 
SbCl5. 

Decomp.  by  H2O.  (Deherain,  C.  R.  52. 
734.) 

4NH4C1,  SbCl5.    Decomp.  by  H2O.    (D.) 

See  also  Chlorantimonate,  ammonium. 

Ammonium    antimony     platinum     chloride, 

(Sb,  Pt)Cl6(NH4)2. 
Ppt.    (Weinland,  B.  1905,  38.  1084.) 

Ammonium  antimony  tin  chloride, 

(Sb,Sn)Cl6(NH4)2. 

Ppt.    (Weinland,  B.  1905,  38.  1085.) 
Ammonium  arsenyl  chloride,  2NH4C1,  AsOCl 


(Wallace,  Phil.  Mag.  (4)  16.  358.) 
Ammonium  bismuth  chloride,  NH4C1,  2BiCl3. 
Deliquescent.    (Deherain,  C.  R.  54.  724.) 
2NH4C1,  BiCl3.  Decomp.  by  H2O.  (Arppe.) 
Pogg.  64.  237.) 

+2>^H2O.    (Rammelsberg.) 

3NH4C1,  BiCl3.  Decomp.  by  H2O.  (Arppe.) 

5NH4C1,  2BiCl3.    (Rammelsberg.) 

Ammonium    bismuth     potassium     chloride, 
2NH4C1,  BiCl3,  KC1. 

(Deherain,  C.  R.  54.  724.)    . 
Ammonium  cadmium  chloride,  NH4C1,  CdCl2. 

Solubilitv  of  NH4C1,  CdCl2  in  H2O  at  t°. 


H 

0.2  §~. 

t° 

Pts.  by  weight  in 
100  pts.  of  solution 

51 

gffl 

^i* 

28 

"^S 

Cl 

Cd 

NH4 

O1""1 

2.4° 

13.44 

14.26 

2.24 

29.94 

42.74 

3.25 

16.0 

15  07 

15.82 

2.56 

33.45 

50.26 

3.83 

41.2 

17  46 

18.61 

2.89 

38.96 

63.83 

4.86 

63.8 

19.73 

20.92 

3.34 

43.99 

78.54 

5.98 

105.9 

23.52 

24.70 

4.01 

52.58 

109  .  33 

8.30 

(Rimbach,  B.  1897,  30.  3076.) 


32 


AMMONIUM  CHLOROMOLYDENUM  CHLORIDE 


SI.  sol.  in  H2O,  alcohol,  and 
wood  spirit,    (v.  Hauer,  W.  A.  B.  13.  449.) 
4NH4C1,  CdCl2.    Sol.  inH2O.    (v.  Hauer.) 
Decomp.  by  H2O  to  NH4C1,  CdCl2.    De- 
comp.  increases  with  decrease  of  temp.    At 
3.9°  approximately  wholly  decomp.  to  NH4C1, 
CdCl2.    At  113.9°  very  nearly  all  is  4NH4C1, 
CdCl2.    (Rimbach,  B.  1897,  30.  3077.) 

Solubility  of  4NH4C1,  CdCl2  in  H2O  at  t°. 


t° 

Pts.  dissolved  in  100  pts.  by 
weight  of  solution. 

Cd 

Cl 

NH4 

3.9 
16.1 
40.2 
58.5 
112.9 
113.9 

5.75 
6.93 
9.91 
12.50 
16.66 
16.51 

18.17 
20.26 
23.84 
26,53 
31.79 
32.71 

7.37 
7.97 
8.92 
9.35 
10.78 
11.30 

Sol.  without  decomp.  in  37.3%  HCl(d  = 
1.19)  and  24.8%  HCl(d  =  1.125).    (Rimbach, 
B.  1905,  38.  1569.) 
Solubility  of  4NH4Cl,CdCl2+NH4Cl  in  H2O 

at  t°. 


In  100  pts.  by  wt.  of  the 
solution 


Composition  of 
the  solid  phase 


Hygroscopic.     Decomp.  by  H2O  and  by 
alcohol.    (Weinland,  B.  1907,  40.  3770.) 
Ammonium  cobaltous  chloride,  NH4C1,  CoCl2 

+6H2O. 

Deliquescent  in  moist  air.    Very  easily  soi. 
in  H2O.    (Hautz,  A.  66.  284.) 
Ammonium    cobaltous    chloride    ammonia, 

NH4C1,  CoGl2,  NH3.    (F.  Rose.) 
Ammonium  cuprous  chloride,  4NH4Cl.Cu2Cl2. 

Decomp.  in  the  air. 

4NH4C1,  3Cu2Cl2.     Decomp.  by  H2O,  not 
by  alcohol.    (Ritthausen,  J.  pr.  59.  369.) 

Fairly  stable  in  air.    (Wells,  Z.  anorg.  1895, 
10.  158.) 
Ammonium  cupric  chloride, 

NH4C1,  CuCl2. 

Solubility  of  NH4C1,  CuCl2  in  absolute  alcohol 
at  25°. 


4.65NH 

4.74 

6.45 


Solid  phase 


4C1+NH4C1, 

CuCl2 
NH4C1+NH4C1, 

CuCl2 
NH4C1,  CuCl2 


12.90 
34.92 
34.50 


Solid  phase 


NH4C1,  CuCl2 

NH4Cl,CuCl2+ 
CuCl2,  C2H5OH 


Pts.  by 
wt.  Cd 


1.0 
13.2 
40.1 

58.2 


2.82 
2.76 
3.16 
3.51 


Pts.  by 
wt.  Cl 


17.11 

18.84 
22.56 
25.21 


Pts.  by 
wt.  NH4 


Mol.  % 
NH4C1 


7.82 

8.71 

10.49 

11.72 


59.0 
74.0 
71.0 
69.0 


Mol.   % 

Tetra- 

salt 


41.0 
26.0 
29.0 
31.0 


(Rimbach,  B.  1902,  36.  1300.) 

Solubility  of  4NH4C1,  CdCl2+NH4Cl,  CdCl2 
in  H2O  at  t°. 


(Foote  and  Walden,  J.  Am.  Ch.  Soc.  1911,  33. 
1032.) 

+2H2O.  Sol.  in  2  pts.  H2O.  (Hautz,  A. 
66.  280.) 

Does  not  exis  t,  (Meerburg,  C.  C.  1904.  II, 
1362. 

2NH4C1,  CuClo  +2H2O.  Easily  sol.  in  H2O, 
also  in  alcohol,  even  when  absolute.  (Cap 
and  Henry,  J.  pr.  13.  184.) 

Solubility  of  2NH4C1,  CuCl2  in  H2O  at  t°. 


In  100  pts.  by  wt.  of  the 

Composition  of 

solution 

the  solid  phase 

t° 

Pts.  by 
wt.  Cd 

Pts.  by 
wt.  Cl 

Pts.  by 
wt.  NH4 

Mol.   % 
Mono- 
salt 

Mol.   % 
Tetra- 
salt 

1.1 

5.34 

17.62 

7.27 

49.6 

50.4 

14.0 

7.12 

19.86 

7.84 

47.0 

53.0 

40.7 

10.24 

23.82 

8.85 

77.0 

23.0 

58.5 

12.50 

26.53 

9.35 

(Rimbach,  B.  1902,  36.  1300.) 
Sol.  without  decomp.  in  50%  LiCl-fAq, 
33.3%    CaCl2+Aq    and    50%    MgCl2+Aq. 
(Rimbach,  B.  1905,  38.  1569.) 

Ammonium  chloromolybdenum  chloride, 

2NH4C1,  Cl4Mo3Cl2+2H20. 
Decomp.  by  pure  H2O;  can  be  crystallized 
from  HCl+Aq.    (Blomstrand.) 

Ammonium    chromium    chloride,    2NH4C1 

CrCl3+H20. 
Sol.  in  H2O  with  decomp.    (Neumann,  A. 

'  +6H25  =  2NH4C1,  [CrCl2.4H20]Cl+2H2O. 


g.  2NH<C1, 
CuCh  in 
100  g.  of  the 
'   solution 

t 

Solid  phase 

3.87 

—1.5° 

ice 

5.88 

—2.48 

8.78 

—3.95 

•  « 

9.97 

—4.60 

14 

13.12 

—6.40 

0 

15.84 

—8.04 

« 

17.64 

—9.24 

«l 

20.12 

—10.80 

«• 

±20.3 

±—11.0 

ice  +2NH4C1,  CuCl2.2H2O 

20.46 

—10 

2NH4C1,  CuCl2.2H2O 

21.16 

—5 

" 

22.02 

0 

ii 

24.26 

+  12 

«« 

25.95 

20 

X 

27.70 

30 

«« 

30.47 

40 

M 

33.24 

50 

<« 

36.13 

60 

II 

39.25 

70 

« 

43.36 

80 

" 

(Meerburg,  Z.  anorg.  1905,  46.  8.) 


AMMONIUM  MOLYBDENUM  CHLORIDE  IODIDE 


33 


Somewhat  sol.  in  liquid  NH3.  (Franklin 
and  Kraus,  Am.  Ch.  J.  1898,  20.  827.) 

Is  the  only  hydrate  of  2NH4C1,  CuCl2  exist- 
ing between  —11°  and  +80°.  (Meerburg, 
C.  C.  1904.  II,  1362.) 

+3H2O.  (Bourgeois,  BuU.  Soc.  1898,  (3) 
19.  786.) 

Ammonium  cupric  chloride  ammonia, 

2NH4C1,  CuCl2,  2NH3. 
Decomp.  by  H2O,  less  easily  by  alcohol. 
Decomp.  by  acids.    (Ritthausen.) 

Ammonium  indium  chloride,  2NH4C1,  InCl3 

+H20. 
Easily  sol.  in  H20.    (Meyer.) 

Ammonium  iodine  chloride,  NH4C1,  IC18. 

More  sol.  in  H2O  than  KC1,  IC13.  (Pilhol, 
J.  Pharm.  25.  441;  Berz.  J.  B.  20.  (2)  110.) 

Ammonium  iridium  trichloride. 
See  Chloriridite,  ammonium. 

Ammonium  iridium  tetracbloride. 
See  Chloriridate,  ammonium. 

Ammonium  iron  (ferrous)  chloride,  NH4C1, 

FeCl2. 

Easily  sol.  in  H20 ;  insol.  in  alcohol.  (Wink- 
ler.) 

Ammonium  iron  (ferric)  chloride,  2NH4C1, 
FeCl3+H20. 

Deliquescent.  Sol.  in  H2O  without  decomp. 
(Fritzsche) ;  sol.  in  3  pts.  H2O  at  18.75°.  (Abl.) 

Sol.  in  H2O.  (Walden,  Z.  anorg.  1894,  1. 
332.) 

Ammonium  iron  (ferric)  potassium  chloride, 

"VTTT    ^11      T     f~**1          TJTi]     I     1  1  ,/TT   /~\ 

JNH4C1,  .beds,  KCl  +  l>^rl2O. 
Min.  Kremersite.     Deliquescent. 

Ammonium  lead  chloride,  NH4C1,  2PbCl2+ 
3H2O. 

Sol.  in  H2O  without  decomp.  (?).  (Andre", 
C.  R.  96.  1502.) 

6NH4C1,  PbCl2+H2O. 

9NH4C1,  PbCl2  +  13^H20. 

9NH4C1,  2PbCl2+2^H2O. 

10NH4C1,  PbCl2+H2O. 

11NH4C1,  2PbCl2+3^H2O. 

18NH4C1,  PbCl2+4H2O. 

All  these  salts  are  decomp.  by  H2O.  (Andre" 
A.  ch.  (6)  3.  104.) 

Of  the  salts  prepared  by  Andre",  only  one 
NH4C1,  2PbCl2  exists.  (Wells,  Sill.  Am.  J. 
146.  25.) 

Solubility  determinations  show  that  NH4C1, 
2PbCl2  is  the  only  double  salt  formed  at  25°. 
(Foote,  Am.  Ch.  J.  1907,  37.  121.) 

NH4C1,  PbCl2  +  V3H20.    (Wells,  Z.c.) 

Ammonium  lead  tefrachloride. 
See  Chloroplumbate,  ammonium. 


Ammonium  magnesium  chloride,  NH4MgCl« 

+6H2O  =  NH4C1,  MgCl2+6H20. 
Deliquescent.    Very  sol.  in  H2O. 
Sol.  in  6  pts.  cold  H2O.    (Fourcroy.) 

Solubility  in  NH4Cl+Aq  at  t°. 


Per  1000  Mol.  H2O 

t°  ' 

Mol. 
NH4C1 

MoL  MgCh 

3.5° 

27.5 

55.7 

25  0 

42.1 

56.4 

50.0 

62.9 

59.1 

(Biltz,  Z.  anorg.  1911,  71.  170.) 

4NH4Cl,5MgCl2+33H20.      Sol.    in    H2O. 
(Berthelot  and  Andre",  A.  ch.  (6)  11.  294.) 

Ammonium    manganous    chloride,    NH4C1, 


Sol.  in  13^  pts.  H20  at  ordinary  temp. 
(Hautz,  A.  66.  280);  does  not  exist.  (Saund- 
ers,  Am.  Ch.  J.  14.  134.) 

2NH4C1,  MnCl2+H2O.  Sol.  in  H2O  (Ram- 
melsberg)  ;  does  not  exist.  (Saunders.) 

+2H2O.  Easily  sol.  in  H2O,  but  with 
decomp.  into  NH4C1  and  MnCl2.  (Saunders.) 

Ammonium  manganic  chloride,  2NH4C1, 
MnCl3. 

Sol.  in  H2O;  less  sol.  in  NH4Cl+Aq.  Un- 
stable. (Neuman,  M.  1894,  16.  490.) 

+H20.  Decomp.  by  H20.  Sol.  in  HC1 
apparently  without  decomp.  (Rice,  Chem. 
Soc.  1898,  73.  260.) 

Ammonium  mercuric  chloride,  2NH4C1, 
HgCl2+H2O  (sal  alembroth). 

Sol.  in  0.66  pt.  H20  at  10°,  and  in  nearly 
every  proportion  of  hot  H2O. 

NH4C1,  HgCl2.    Easily  sol.  in  H20. 

+  ^H2O.    Easily  sol.  in  H2O.    (Kane.) 

2NH4C1,  3HgCl2+4H2O.  Easily  sol.  in 
H2O.  (Holmes,  C.  N.  6.  351.) 

NH4C1,  2HgCl2.  Very  sol.  in  H2O.  (Ray, 
Chem.  Soc.  1902,  81.  648.) 

NH4C1,  5HgCl2.  (Stromholm,  J.  pr.  1902, 
(2)  66.  441.) 

Ammonium  mercuric  sodium  chloride,  NH4C1, 

HgCl2,  4NaCl  (?). 

Sol.  in  H2O.  (Kossmann,  A.  ch.  (3)  27. 
243.) 

Ammonium  molybdenum  chloride,  2NH4C1, 
MoCl3+H2O. 

Very  sol.  in  H20.  Nearly  insol.  in  alcohol 
and  ether.  (Chilesotti,  C.  C.  1903.  II,  652.) 

/See  also  Ammonium  chloromolybdenum 
chloride. 

Ammonium  molybdenum  chloride  iodide. 
See  Ammonium  chloromolybdenum  iodide. 


34 


AMMONIUM  MOLYBDENYL  CHLORIDE 


-Ammonium  molybdenyl   chloride,   2NH4C1, 

Mo02Cl2+2H2O. 

(Weinland,  Z.  anorg.  1905,  44.  98.) 
2NH4C1,  MoOCl3.    Sol.  in  H2O;  insol.  in 
H2O  sat.  with  HC1.     (Klason,  B.  1901,  34. 
149. 

Ammonium  nickel  chloride,  NH4C1,  NiCl2  + 
6H20. 

Deliquescent  in  moist  air.  Easily  sol.  in 
H2O.  (Hautz.) 

4NH4C1,  NiCl2+7H2O  (?). 

Ammonium  osmium  tetrachlonde. 
See  Chlorosmate,  ammonium. 

Ammonium  osmium  sesgm'chloride. 
See  Chlorosmite,  ammonium. 

Ammonium  osmyl  chloride,  (NH4)2OsO2Cl4. 

Sol.  in  H2O.  Decomp.  by  HC1.  (Wintre- 
bert,  A.  ch.  1903,  (7)  28.  92.) 

Ammonium  osmyl  oxy chloride, 

(NH4)2Os03Cl2. 

Very  si.  sol.  in  H20.  Sol.  in  KOH+Aq 
with  decomp.  (Wintrebert,  A.  ch.  1903,  (7) 
28.  116.) 

Ammonium  palladium  chlorides. 

See  Chloropalladate,  ammonium  and  chloro- 
palladite,  ammonium. 

Ammonium  rhodium  bichloride,  4NH4C1, 
RhCl2+3^H2O. 

Sol.  in  H20,  but  decomp.  slowly.  (Willm. 
B.  16.  3033.) 

Does  not  exist.    (Leidie,  A.  ch.  (6)  17. 277.) 

Ammonium  rhodium  trichloride. 
See  Chlororhodite,  ammonium. 

Ammonium  rhodium  chloride  ammonium 
nitrate,  Rh2Cl6,  6NH4C1,  2NH4NO3. 

See  Chlororhodite  nitrate,  ammonium. 
Ammonium  ruthenium  trichloride. 

See  Chlororuthenite,  ammonium. 
Ammonium  ruthenium  tefrachloride. 

See  Chlororuthenate,  ammonium. 
Ammonium  tellurium  chloride. 

See  Chlorotellurate,  ammonium. 
Ammonium  thallic  chloride,  3NH4C1,  T1C13. 

Easily  sol.  in  H2O.    (Wilhn.) 

+2H2O.  Easily  sol.  in  H2O  and  alcohol. 
(Nickles,  J.  Pharm.  (4)  1.  28.) 

Ammonium  thorium  chloride,  8NH4C1,  ThCL 

+8H20. 
Sol.  inH20.    (Chydenius.) 

Ammonium  tin  (stannous)  chloride  (ammon- 
ium chlorostannite),  NH4C1,  SnCl2+H2O. 
Decomp.    by    H2O.      Resembles   K    salt 
(Richardson,  Am.  Ch.  J.  14.  93.) 


2NH4C1,  SnCl2+H2O.  Sol.  in  H2O,  but 
decomp.  by  boiling.  (Rammelsberg.) 

Contains  2H2O.    (Richardson.) 

4NH4C1,  SnCl2+3H2O.  Decomp.  by  H,O. 
(Poggiale,  C.  R.  20.  1182.) 

Does  not  exist.    (Richardson.) 

Ammonium  tin  (stannic)  chloride. 
See  Chlorostannate,  ammonium. 

Ammonium  titanium  chloride,  2NH4C1,  TiCl4 

-t-2H20. 

Ppt.;  decomp.  in  moist  air;  sol.  in  fuming 
HC1;  insol.  in  ether.  (Rosenheim,  Z.  anorg. 
1901,  26.  242.) 

Ammonium  titanium  chloride,  3NH4C1,  TiCl4. 
Sol.  in  H2O. 
6NH4C1,  TiCl4.    Sol.  inH2O.    (Rose.) 

Ammonium  tungsten  chloride,  (NH4)3W2C19  = 

3NH4C1,  2WC13. 

Easily  sol.  in  H2O.  Nearly  insol.  in  most 
organic  solvents.  (Olsson,  B.  1913,  46.  577.) 

Ammonium  uranyl  chloride. 

Very  deliquescent,  and  sol.  in  H2O.  (Peli- 
got.) 

2NH4C1,(UO2)C12+2H2O.  Solution  at  15° 
contains  in  100  g.  3.51  g.,  NH4,  40.67  g.  UO2 
and  19.15  g.  Cl,  hence  there  is  considerable 
decomp.  (Rimbach,  B.  1904,  37.  466.) 

Ammonium    vanadium    chloride,    2NH4C1. 

VC13+H2O. 

Difficulty  sol.  in  H2O  and  alcohol.  (Stabler, 
B.  1904,  37.  4412.) 

Ammonium  zinc  chloride,  NH4C1,  ZnCl2-f- 
2H2O. 

Deliquescent.  Very  sol.  in  H2O.  (Hautz, 
A.  66.  287.) 

2NH4C1,  ZnCl2.  Sol.  in  H2O.  (Rammels- 
berg, Pogg.  94.  507.) 

+H2O.  Deliquescent  in  moist  air.  Sol.  in 
2/a  pt.  cold  H2O  with  absorption  of  heat.  Sol. 
in  0.28  pt.  hot  H2O  (Golfier-Bassayre,  A. 
ch.  70.  344) ;  sol.  in  1A  pt.  cold  H2O.  (Hautz, 
A.  66.  287.) 

3NH4C1,  ZnCl2.    Sol.  in  H2O.    (Marignac.) 

+H2O.    (Berthelot,  A.  ch.  (6)  11.  294.) 

4NH4C1,  ZnCl2.    (Deh6rain.) 

6NH4C1,  ZnCl,+ViH,0.    (Berthelot,  I.e.) 

Ammonium  chloride  zinc  oxychloride,  2ZnCl2, 
8NH4C1,  ZnO. 

Sol.  in  a  little  H2O,  but  decomp.  by  excess. 
(Andre.) 

3ZnCl2, 10NH4C1,  ZnO.  As  above.  (Andre, 
A..ch.  (6)3.88.) 

Ammonium  chloride  antimony  fluoride. 
NH4C1,  SbF3. 

Easily  sol.  in  H20.  (de  Haen,  B.  21. 901  R.) 
Ammonium  chloride  arsenic  inoxide. 

See  Arsenite  chloride,  ammonium. 


AMMONIUM  MANGANIC  FLUORIDE 


35 


e, 


Ammonium  chloride  bismuth  bromide. 
3NH4C1,  BiBr3+H2O. 

Deliquescent;  decomp.  by  H2O.  (Muir, 
Chem.  Soc.  31.  148.) 

2NH4C1,  BiBr3+3H2O.  Decomp.  by  H2O. 
(Muir.) 

5NH4C1,  2BiBr3+H2O.  Decomp.  by  H2O. 
(Muir.) 

Ammonium    chloride    chromic    oxychloride. 

2NH4C1,  CrOCl3. 

Decomp.  in  the  air.  Sol.  in  cone.  HC1 
without  decomp.  (Weinland,  B.  1906,  39. 
4045.) 

Ammonium  chloride  cuprocupric  thiosulphat 

2NH4C1,  Cu2O,  CuO,  3S2O2. 
See    Thiosulphate     ammonium    chloride, 
cuprocupric. 

Ammonium  chloride  lead  iodide.  3NH4C1, 
PbI2. 

Decomp.  with  H->O.  (Behrens,  Pogg.  62. 
252.) 

4NH4C1,  PbIo+2H2O.  Decomp.  with  H20. 
(Poggiale,  C.  R.  20.  1180.) 

Ammonium     chloride     mercuric     bromide. 

NH4Ci,  HgBr2. 
(Edhem-Bey,  Dissert.  1885.) 

Ammonium  chloride  platinum  sulphite. 
See  Chloroplatosulphite,  ammonium. 

Ammonium  chloride  tin  (stannous)  bromide, 

2NH4C1,  SnBr2+H2O. 
Sol.  in  H2O.    (Raymann  and  Preis,  A.  223. 
323.) 

Ammonium  cfo'chloroiodide,  NH4Cl2l. 

Slowly  decomp.  when  exposed  to  dry  air 
at  ord.  temp.  Very  sol.  in  H2O.  (Chattaway, 
Chem.  Soc.  1915,  107.  107.) 

Ammonium  tefrachloroiodide,  NH4C14I. 

Decomp.  in  the  air.  (Chattaway,  Chem. 
Soc.  1915,  107.  107.) 

Ammonium  lead  chloroiodide,  NH4PbClI2  + 

2H20  and  (NH4)2PbCl2I2+2H2O. 
Sol.  in  KOH+Aq  and  in  strong  acids;  de- 
comp. by  H2O.     (Fonzes-Diacon,  Bull.  Soc. 
1897,  (3)  17.  348.) 

Ammonium  fluoride,  NH4F. 

Abundantly  sol.  in  H2O;  si.  sol.  in  alcohol. 
(Marignac,  Ann.  Min.  (5)  15.  221.) 

Insol.  in  liquid  NH3.  (Ruff  and  Geisel,  B. 
1903,  36.  820.) 

Almost  insol.  in  liquid  NH»  at  50°.  (Mois- 
san,  C.  R.  1901,  133.  713.) 

Sol.  in  methyl  alcohol.  (Carrara,  Gazz. 
ch.  it.  1896,  26.  119.) 

Ammonium  hydrogen  fluoride,  NH4F,  HF. 
Deliquescent  in  moist  air.    Sol.  in  H2O. 


Ammonium  antimony  fluoride,  2NH4F,  SbF3. 

Deliquescent;  sol.  in  0.9  pt.  cold  H2O. 
Insol.  in  alcohol  or  ether.  (Fluckinger,  A. 
84.  248.) 

NH4F,  4SbF3.    3  pts.  sol.  in  2  pts.  H2O. 

(Raad  and  Hauser,  B.  1890,  23.  R.  125.) 

NH4F,  SbF5.  Easily  sol.  in  H2O.  (Marig- 
nac, A.  145.  239.) 

Ammonium  bismuth  fluoride,  2NH4F,  BiF3. 

Insol.  in  H2O.  Rather  difficultly  sol.  in 
acids.  (Helmholt,  Z.  anorg.  3.  115.) 

Ammonium  cadmium  fluoride,  NH4F,  CdF2. 
Insol.  in  H2O.     Sol.  in  acids  on  boiling. 
(Helmholt,  Z.  anorg.  3.  115.) 

Ammonium  chromium  fluoride,  3NH4F, 
CrF3. 

Easily  sol.  in  H2O.    SI.  sol.  in  NH4F+Aq. 
(Petersen,  J.  pr.  (2)  40.  52.) 
2NH4F,CrF3+H2O.     (Wagner,  B.  19. 896.) 

Ammonium  cobaltous  fluoride,  2NH4F,  CoF2 

+2H20. 

SI.  sol.  in  H2O.    (Wagner,  B.  19.  896.) 
Easily  sol.  in  H-O.     (Helmholt,  Z.  anorg. 

3.  132.) 

Ammonium  columbyl  fluoride. 
See  Fluoxycolumbate,  ammonium. 

Ammonium  columbium  fluoride  oxyfluoride, 

3NH4F,  CbF6,  CbOF3. 
See  Fluoxycolumbate  columbium  fluoride, 
ammonium. 

Ammonium  copper  fluoride,  2NH4F,  CuF2  + 
2H20. 

Insol.  in  H2O.  (Helmholt,  Z.  anorg.  3. 
115.) 

Nearly  insol.  in  H2O  but  decomp.  thereby. 
(Haas,  Ch.  Z.  1908,  32.  8.) 

Ammonium  glucinum  fluoride,  2NH4F,  G1F2. 
Sol.  in  H2O.  (Marignac,  A.  ch.  (4)  30.  51.) 
Very  sol.  in  H2O.  (Helmholt,  Z.  anorg.  3. 

130.) 

Ammonium  iron  (ferrous)  fluoride,  2NH4F, 

FeF2.     (Wagner,  B.  19.  896.) 
NH4F,  FeF2-f-2H2O.    (W.) 

Ammonium  iron  (ferric)  fluoride,  2NH4F, 
FeF3. 

More  sol.  in  H2O  than  the  corresponding  K 
compound.  Decomp.  by  boiling.  (Nickles, 
J.  Pharm.  (4)  7.  15.) 

3NH4F,  FeF8.  SI.  sol.  in  H20.  (Marignac, 
A.  ch.  (3)  60.  306.) 

EasUy  sol.  in  acids.  (Helmholt,  Z.  anorg. 
3.  124.) 

Ammonium     manganic     fluoride,     2NH4F, 

MnF4. 

More  sol.  than  the  K  salt.  (Nickles,  C.  R 
65.  107.) 


36 


AMMONIUM  MANGANYL  FLUORIDE 


True  Composition  is  4NH4F,  Mn2F6.  (Chris- 
tensen,  J.  pr.  (2)  34.  41.) 

See  also  Fluomanganate,  ammonium. 
Ammonium  manganyl  fluoride. 

See  Fluoxymanganate,  ammonium. 
Ammonium  molybdenum  fluoride. 

Insol.  in  H2O.  Sol.  in  HCl+Aq.  (Berze- 
lius.) 

See  also  Fluomolybdate,  ammonium. 
Ammonium  molybdenyl  fluoride. 

See  Fluoxymolybdate,  ammonium. 

Ammonium  nickel  fluoride,  2NH4F,  NiF2+ 

2H20. 

Sol.  in  H2O.    (Wagner,  B.  19.  896.) 
Easily  sol.  in  H2O.    (Helmholt,  Z.  anorg.  3. 

143.) 

Ammonium  scandium  fluoride,  (NH4)3ScF6. 

Easily  sol.  in  H2p.  Aqueous  solution  is  liot 
decomp.  by  boiling.  Decomp.  by  acids. 
(R.  I.  Meyer,  Z.  anorg.  1914,  86.  275.) 

Ammonium  silicon  fluoride. 
See  Fluosilicate,  ammonium. . 

Ammonium  silver  fluoride,  2NH4F,  AgF+ 
H2O. 

Not  hydroscopic.  Sol.  in  H2O;  sol.  in  cone. 
NH4F+Aq.  Sol.  in  alcohol.  (Griitzner, 
Arch.  Pharm.  1900,  238.  3.) 

15NH4F,  AgF+4H2O.  More  deliquescent 
than  NH4F.  (Bohm,  Dissert.  1906.) 

Ammonium  tantalum  fluoride. 

See  Fluotantalate,  ammonium. 
Ammonium  tantalyl  fluoride. 

See  Fluoxytantalate,  ammonium. 
Ammonium  tellurium  fluoride,  NH4F,  TeF4. 

Decomp.  by  H20.  (Hogbom,  Bull.  Soc.  (2) 
35.  60.) 

Ammonium  tin  (stannous)  fluoride,  2NH4F, 

SnF2+2H2O. 
Sol.  in  H2O.    (Wagner,  B.  19.  896.) 

Ammonium  tin  (stannic)  fluoride,  2NH4F, 

SnF4. 

See  Fluostannate,  ammonium. 
Ammonium  titanium  sesquifiuonde. 

See  Fluotitanate,  ammonium. 
Ammonium  titanyl  fluoride. 

See  Fluoxypertitanate,  ammonium. 
Ammonium  tungstyl  fluoride. 

See  Fluoxytungstate,  ammonium. 
Ammonium  uranyl  fluoride. 

See  Fluoxyuranate,  ammonium. 
Ammonium  vanadium  ses^mfluoride. 

See  Fluovanadate,  ammonium. 


Ammonium  vanadyl  fluoride. 
See  Fluoxyvanadate,  ammonium. 

Ammonium  zinc  fluoride,  2NH4F,  ZnF2. 

Sol.  inH20.    (R.  Wagner.) 

+2H2O.  Very  si.  sol.  in  H2O.  Easily  sol. 
in  dil.  acids.  (Helmholt.) 

Ammonium  zirconium  fluoride. 
See  Fluozirconate,  ammonium. 

Ammonium  fluoride  manganic   oxyfluoride, 

2NH4F,  MnOF2. 
Precipitate.    (Nickles.) 
See  also  Fluoxymanganate,  ammonium. 

Ammonium   fluoride  molybdenum  dioxide, 

2NH4F,  Mo03. 

Decomp.  by  H2O.  (Mauro.  Gazz.  ch.  it. 
18.  120.) 

Ammonium  fluoride  tungsten  oxyfluoride. 
See  Fluoxytungstate,  ammonium. 

Ammonium  fluoride  tungsten  oxyfluoride 
ammonium  tungstate,  4NH4F,  WO2F2, 
(NH4)2W04. 

See  Fluoxytungstate  tungstate,  ammonium. 
Ammonium  fluoride  vanadium  oxyfluoride. 

See  Fluoxyvanadate,  and  fluoxyhypovana- 
date,  ammonium. 

Ammonium  hydroselenide,  NH4HSe. 

Sol.  in  H2O  with  decomp.  (Bineau,  A.  ch. 
(2)  67.  229.) 

Ammonium  hydrosulphide,  NH4SH. 

Sol.  in  H20  and  alcohol.  Solutions  decomp. 
on  air. 

Ammonium  hydroxide,  NH4OH. 
See  Ammonia, 

Ammonium    imidosulphamide, 

(S2O4N3H4)NH4. 
(Hantzsch,  B.  1905,  38.  1033.) 

Ammonium  iodide,  NH4I. 

Very  deliquescent.  Sol.  in  0.60  pt.  H2O. 
(Eder,  Dingl.  221.  89.) 

Sp.  gr.  of  aqueous  solution  of  NH4I  at  18° 
containing — 

10          20          30          40          50%NH4I. 
1.0652  1.1397  1.2260  1.3260  1.4415 
(Kohlrausch,  W.  Ann.  1879.  1.) 

NH4I+Aq  containing  12.51%  NHJ  has 
sp.gr.  20°/20°  =  1.0846. 

NH4I+Aq  containing  19.19%  NHJ  has 
sp.  gr.  20°/20°  =  1.1359. 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 

Very  easily  sol.  in  liquid  NH3.  (Franklin 
Am.  Ch.  J.  1898,  20.  826.) 

Very  sol.  in  liquid  NH3  at  — 50°.  (Moissan, 
C.  R.  1901,  133.  713.) 


AMMONIUM  ZINC  IODIDE 


37 


Sol.  in  SOC12.  (Walden,  Z.  anorg.  1900, 
25.  216.) 

Sol.  in  liquid  SO2.  (Walden,  Z.  anore. 
1902,  30.  160.) 

Sol.  in  4.0  pts.  abs.  alcohol.    (Eder,  I.e.} 
"  210    "    ether.    (Eder,  I.e.) 
"    20     "     alcohol-ether  (1  :  1).  (Eder, 
l.c-.) 

Sol.  in  acetone.  (Eidmann,  C.C.  1899,  II. 
1014.);  (Naumann,  B.  1904,  37.  4328.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  "314.) 

SI.  sol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1369.) 

Ammonium  (Modide,  NH4I2. 

Sol.  in  alcohol,  ether,  CS2,  and  KI+Aq; 
less  sol.  in  chloroform.    (Guthrie,  Chem.  Soc. 
(2)  1.  239.) 
Ammonium  imodide,  NHJs. 

SI.  deliquescent.  Sol.  in  little  H2O,  but 
decomp.  by  much  H2O.  (Johnson,  Chem. 
Soc.  33.  397.) 

Ammonium  antimony  iodide,  NH4I,  SbI3  + 
2H2O. 

Decomp.  by  H2O.  (Nickles,  C.  R.  51. 
1097.) 

3NHJ,  4SbI3+9H2O.  Decomp.  by  H20, 
with  separation  of  SbOI.  Sol.  in  HC2H3O2, 
HC1,  and  H2C4H4O6+Aq.  Decomp.  by  CS2. 
(Schaffer,  Pogg.  109.  611.) 

3NH4I,  SbI3+3H2O.    As  above. 

4NHJ,  SbI3+3H2O.    As  above. 

Ammonium  bismuth  iodide,  NH4I,  BiI3  + 
H20. 

Deliquescent;  decomp.  by  H2O.  (Nickles, 
C.  R.  51.  1097.) 

4NHJ,  BiI3+3HoO.  As  above.  (Linau, 
Pogg.  111.  240.) 

2NHJ,  BiI3+2KH2O.  Decomp.  by  H2O, 
or  MCI,  MBr,  or  MI+Aq.  (Nickles,  J.  pr 
(2)  39.  116.) 

Ammonium  cadmium  iodide,  2NH4I,  CdI2  + 
2H2O. 

Deliquescent.    (Croft.) 

Sol.  at  15°  in  0.58  pt.  H2O,  0.70  pt.  abs. 
alcohol.,  8.9  pts.  ether  (sp.  gr.  0.729),  and 
1.8  pts.  alcohol-ether  (1:1).  (Eder,  Dingl 
221.  89.) 

100  pts.  of  the  solution  in  H20  contain  85.91 
pts.  of  the  salt  at  14.5°.  (Rimbach,  B.  1905 
38.  1563.) 

NH4I,  CdI2+HH20.  Sol.  at  15°  in  0.90 
pt.  H2O,  0.88  pt.  abs.  alcohol,  and  2.4  pts 
ether  (sp.  gr.  0.729).  (Eder,  l.c.) 

+H2O.  (Grossmann,  Z.  anorg.  1902,  33 
154.) 

Ammonium  chloromolybdenum  iodide, 
2NH4I,  Cl4Mo3I2+2H20. 

Decomp.  by  H2O.  Cryst.  from  HI+Aq. 
(Blomstrand.) 


Ammonium  cuprous  iodide,  2NH4I,  Cu2I2  + 

H2O. 

Decomp.  on  the  air,  or  by  H2O,  or  alcohol. 
Saglier,  C.  R.  104.  1440.) 

-J-KH2O.  Decomp.  by  H2O  with  separa- 
tion of  Cu2I2.  (Gossner,  Zeit.  Kryst.  1903,  38. 
501.) 

Ammonium  cupric  iodide  ammonia,  2NH4I, 
CuI2,  2NH3+2H20. 

Insol.  in  H2O  or  alcohol;  si.  sol.  in  NH4OH 
+Aq. 

+6H2O.  Unstable.  (Saglier,  C.  R.  104. 
1440.) 

NH4I,  2CuI2,  3NH3.  (Fleurent,  C.  R. 
1891,  113.  1047.) 

Ammonium  iridium  (Modide,  2NH4I,  IrI2. 

Insol.  in  cold  or  hot  H2O,  and  in  alcohol. 
Sol.  in  warm  dil.  acids.  (Oppler.) 

Ammonium  iridium  sesgmiodide. 
See  lodiridite,  ammonium. 

Ammonium  iridium  tefraiodide. 
See  lodiridate,  ammonium. 

Ammonium  lead  iodide,  NH4I,  PbI2+2H2O. 

Decomp.  by  much  H20.  (Wells,  Sill.  Am. 
J.  146.  25.) 

4NHJ,3PbI2+6H2O.  SI.  sol.  in  H20. 
(Mosnier,  C.  R.  1895,  120.  444.) 

Sol.  in  H20  with  decomp.  Sol.  in  strong 
KOH+Aq  and  in  strong  acids.  (Fonzes- 
Diacon,  Bull.  Soc.  1897,  (3)  17.  347.) 

Ammonium  magnesium  iodide,  NH4I,  MgI2 
+6H2O. 

Very  deliquescent.  (Lerch,  J.  pr.  (2)  28. 
338.) 

Ammonium  mercuric  iodide,  NHJ,  HgI2  + 
H2O. 

Decomp.  into  its  constituents  by  H2O. 
(Boullay,  A.  ch.  (2)  34.  345.) 

Sol.  without  decomp.  in  alcohol  and  ether. 

NHJ,  2HgI2.  Decomp.  by  H2O.  Sol.  in 
KI+Aq.  Very  sol.  in  alcohol,  ether  and 
nitrobenzol.  (Low,  Zeit.  Kryst,  51.  138.) 

Ammonium  silver  iodide,  2NH  J,  Agl. 

Deliquescent.  Decomp.  by  H2O.  (Pog- 
giale.) 

Ammonium  thallic  iodide,  NHJ,  T1I3. 

Sol.  in  H2O.    (Nickles,  J.  Pharm.  (4)  1.  32.) 

Ammonium  tin  (stannous)  iodide,  NHJ,  SnI2. 

Decomp.  by  small  amt.  H2O  but  completely 
sol.  in  a  large  amt.  (Boullay,  A.  ch.  (2)  34. 
376.) 

+  1KH2O.    (Personne.) 

Ammonium  zinc  iodide,  2NH  J,  ZnI2. 

Extremely  deliquescent,  and  sol.  in  H2O. 
(Rammelsberg,  Pogg.  43.  665.) 


38 


AMMONIUM  IODIDE  ARSENIC  OXIDE 


NHJ,  ZnI2+4^H2O.  Hydroscopic. 
(Ephraim,  Z.  anorg.  1910,  67.  384.) 

Ammonium  iodide  arsenic  trioxide. 
See  Arsenite  iodide,  ammonium. 

Ammonium  cobalt  nitride. 

See  Ammonium  cobalt  azoimide. 

Ammonium  ruthenium  cfohydronitrosobrom- 

ide,  NO.Ru2H2(NH3)6Br3.2HBr. 
Ppt.    (Brizard,  A.  ch.  1900,  (7)  21.  363.) 

Ammonium  ruthenium  nitrosochloride, 

3NH4C1.2HCl.NORu2H2Cl3. 
Ppt.    (Brizard,  A.  ch.  1900,  (7)  21.  354.) 

Ammonium  ruthenium  dihydronitrosochlor- 

ide,  NO.Ru2H2(NH3)6Cl3.2HCl. 
Ppt.    (Brizard,  A.  ch.  1900,  (7)  21.  358.; 

Ammonium  peroxide,  (NH4)2O2. 

M.-pt.  —2°.  SI.  sol.  in  ether  without 
decomp.  (D'Ans,  B.  1913,  46.  3076.) 

Sol.  in  alcohol;  insol.  in  ether;  decomp. 
slowly  in  aq.  solution.  (Melikoff,  B.  1897,  30. 
3145.) 

Ammonium  hydrogen  peroxide,  (NH4)2O2, 
H2O2. 

Decomp.  at  ordinary  temp.  (Melikoff,  B. 
1898,  31.  447.) 

-fH2O.  Unstable;  deliquesces  at  ordinary 
temp.;  sol.  in  alcohol;  insol.  in  light  petroleum. 
(Melikoff,  B.  1898,  31.  152.) 

Ammonium  selenide,  (NH4)2Se. 

Sol.  in  H2O  with  decomp.  (Bineau,  A.  ch. 
(2)  67.  229.) 

Stable  in- the  air.  Sol.  in  H2O;  aq.  solution 
decomp.  slowly.  (Lenher  and  Smith,  J.  Am. 
Chem.  Soc.  1898,  20.  277.) 

Ammonium  hydrogen  selenide,  NH4HSe. 
Sol.  in  H2O.    (Fabre,  C.  R.  103.  269.) 

Ammonium  raonosulphide,  (NH4)2S. 

Decomp.  on  air.  Sol.  in  H2O,  but  solution 
decomposes  rapidly. 

Very  sol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  826.)  ' 

Ammonium  disulphide,  (NH4)2S2. 

Sol.  in  H2O  with  decomp. 

Does  not  exist.  (Bloxam,  Chem.  Soc. 
1895,  67.  293.) 

Ammonium  tefrasulphide,  (NH4)2S4. 

Easily  sol.  in  H2O.  Cone,  solution  is  stable, 
dil.  solution  decomp.  on  air.  Easily  sol.  in 
alcohol  without  decomp.,  but  solution  de- 
comp. on  the  air  more  rapidly  than  the 
aqueous  solution.  (Fritzsche,  J.  pr.  32.  313.) 

+  KH2O.  When  dissolved  in  H2O,  it  is  at 
once  dissociated  with  deposition  of  S.  (Blox- 
am, Chem.  Soc.  1895,  67.  303.) 


Ammonium  pen/asulphide,  (NH4)2S5. 

Decomp.  on  air.  Sol.  in  H20  with  separa- 
tion of  S.  Sol.  in  alcohol  without  decomp., 
but  solution  decomposes  quickly  on  standing. 
(Fritzsche,  J.  pr.  32.  313.) 

Rapidly  decomp.  by  H2O  with  separation 
of  S.  (Bloxam,  Chem.  Soc.  1895,  67.  298.) 

+H2O.  Decomp.  by  H<>O  with  separation 
of  S.  (Bloxam,  Chem."  Soc.  1895,  67.  298.) 

Ammonium  fteptasulphide,  (NH4)2S7. 

More  stable  on  air,  and  less  easily  decom- 
posed by  H2O  than  (NH4)2S6. 

+  lVsH2O.  Decomp.  by  H2O  with  separa- 
tion of  S.  Slowly  attacked  by  dil.  HCl+Aq. 
(Bloxam,  Chem.  Soc.  1895,  67.  307.) 

T^rammonium    hepta  sulphide,     (NH4)4S7  + 

4H2O. 

Sol.  in  H2O.  Solution  can  be  kept  for  a 
long  time  without  depositing  S.  (Bloxam, 
Chem.  Soc.  1895,  67.  298.) 

Diammonium      ennea  sulphide,      (NH4)2S9+ 


Decomposed  by  H2O  with  separation  of  S. 
Not  attacked  by  boiling  dil.  HCl+Aq  on 
account  of  formation  of  a  hard  crust  of  S 
on  the  crystals.  (Bloxam,  Chem.  Soc.  1895. 
67.  306.) 

Teirammonium  enneasulphide,  (NH4)4S9. 

Solution  in  H2O  deposits  crystals  of 
(NH4)2S5  on  standing.  (Bloxam,  Chem.  Soc. 
1895,  67.  302.) 

+3HH2O.  Decomp.  by  H2O  with  separa- 
tion of  S.  (Bloxam,  Chem.  Soc.  1895,  67. 
299.) 

Ammonium  po^sulphides. 

Cone.  NH3+Aq  dissolves  H2S  to  form 
(NH4)2S,2NH4SH.  On  dilution  more  H2S  is 
absorbed  to  form  (NH4)2S,4NH4SH,  then 

(NH4)2S,8NH4SH,  then  (NH4)2S,18NH4SH 
and  finally  NH4SH.  (Bloxam,  Chem.  Soc. 
1895,  67.  284.) 

Ammonium      copper      sulphide,      (NH4)2S, 
2CuS3  (?). 

Sol.  in  warm  H2O,  but  decomp.  on  standing. 
Warm  KOH+Aq  acts  similarly;  si.  sol.  in 
NH4OH+Aq,  Na2CO3+Aq,  or  absolute  al- 
cohol. Insol.  in  ether.  Decomp.  by  dil  acids 

riwoznik,  B.  6.  1291.) 

Correct  formula  is  NH4CuS4.     SI.  sol.  in 
H2p.      Decomp.    by    cone,    and    dil.    acids. 
Easily  sol.  in  NaOH.     SI.   sol.  in  alcohol 
Biltz,  B.  1907,  40.  976.) 

Ammonium  gold  pofysulphide,  AuS3NH4. 

Ppt.     (Hofmann,  B.   1903,   36.  3092-  B 
1904,  37.  245.) 

Ammonium  iridium  pentadecasulphide, 

IrSl5(NH4)3. 

Ppt.    (Hofmann,  B.  1904,  37.  247.) 


ANTIMONIC  ACID 


39 


Ammonium  palladium  imrfecasulphide. 


Ppt.     (Hofmann,  B.  1904,  37.  248.) 

Ammonium    platinum    pentadecasulphide, 

PtS16(NH4)2+2H20. 

Can  be  washed  with  CS2  without  decomp. 
Sol.  in  alcohol.  Insol.  in  ether.  (Hofmann, 
B.  1903,  36.  3091.) 

Ammonium  stannic  sulphide. 
See  Sulphostannate,  ammonium. 

Ammonium  telluride,  NH4HTe. 

Easily  sol.  in  H2O.    (Bineau,  A.  ch.  (2)  67. 

229.)' 

Ammonium    sulphide    ammonia.     (NH4)2S, 

2NH3. 

Very  unstable.  (Bloxam,  Chem.  Soc.  1895, 
67.  294.) 

Ammonium    acz'sulphomelid,    (NSO.ONH4)3 

(?)• 
(Hantzsch  and  Stuer,  B.  1905,  38.  1039.) 

AmmonplatinrJ/amine  comps. 
See  Platin^n'amine  comps. 

Ammoncfa'sulphonic  acid,  NH3(S03H)2. 

Known  only  in  its  salts.  (Claus,  A.  158. 
52  and  194.) 

Contains  2  at.  H  less,  and  is  identical  with 
imidosulphonic  acid  NH(SOsH)2,  which  see. 
(Raschig,  A.  241.  161.) 

Ammonin'sulphonic  acid,  NH2(S03H)3. 

Known  only  in  its  salts.  (Claus,  A.  158. 
52  and  194.) 

Contains  2  at.  H  less,  and  is  nitrilosulphonic 
acid  N(SO3H)3,  which  see.  (Raschig,  A.  241. 
161.) 

Ammontoasulphonic  acid,  NH(SO3H)4. 

Known  only  in  its  salts.  (Claus,  A.  168. 
52  and  194.) 

Does  not  exist,  but  was  impure  nitrilosul- 
phonic acid,  which  see.  (Raschig,  A.  241. 
161.) 

Anhydroarseniotungstic  acid, 
See  under  Arseniotungstic  acid. 

Anhydrooxycobaltamine  chloride, 

Co2(NH3)10  [0(OH)1 

Easily  sol.  in  H2O,  but  decomposes  after  a 
few  minutes;  can  be  recrystallized  from  dil. 
HCl+Aq.  Precipitated  from  sat.  H2O  solu- 
tion by  cone.  HCl+Aq,  or  alcohol.  (Vort- 
mann,  M.  Ch.  6.  404.) 

Co2(NH3)10 
mann.) 


Anhydrooxycobaltamine    chloride    mercuric 

chloride,  Co2(NH3)10(C102H)Cl4,  3HgCl2. 

Can  be  recryst.  from  very  dil.  hot  HCl+Aq. 

chloroplatinate,  Co2(NH8)io(ClO2H)Cl4, 

2PtCl4. 

Can  be  recrystallized  from  H2O  containing 
HC1. 

— —  chloronitrate, 

Co2(NH3)10Cl(O.OH)(N03)4+H20. 

Can  be  recrystallized  from  dil.  HCl+Aq. 

Co2(NH3)10Cl(O.OH)Cl2(N03)2+H2O. 
More  easily  sol.  in  H2O  than  the  preceding 
comp. 

chlorosulphate, 

Co2(NH3)10Cl(O.OH)(S04)2. 

cftchromate,  [Co2(NH3)10O.OH]2(Cr207)5 

+8H2O. 
SI.  sol.  in  H2O. 

nitrate,  Co2(NH3)10(NO3)(O.OH)(NO3)4 

+H20. 

SI.  sol.  in  pure  H2O  with  immediate  decomp. 
Can  be  recrystallized  from  H2O  containing 
HNO3. 

sulphate,       [Co2(NH3)10O  .  OH]2(SO4)6, 

2H2SO4+2H2O. 

SI.  sol.  in  cold  H2O.  When  crystallized 
from  dil.  H2SO4+Aq,  is  converted  into — 

[Co2(NH3)10O.OH]2(S04)6,H2S04+3H20, 
which  by  further  recrystallization  from  very 
dil.  H2SO4+Aq  becomes — 

[Co2(NH3)10O.OH]2(SO4)5+8H2O.  SI.  sol. 
in  cold  H2O.  (Vortmann.) 

Anhydrophospholuteotungstic  acid, 

H3PW8028. 
See  under  Phosphotungstic  acid. 

Antimonic  Acid. 
Mefantimonic  acid,  HSb03. 

Very  si.  sol.  in  H2O;  sol.  in  cone.  HCl+Aq; 
si.  sol.  in  dil.  HNO3+Aq;  easily  sol.  in  tar- 
taric  acid+Aq;  easily  sol.  in  hot  KOH,  or 
NaOH+Aq;  completely  insol.  in  NH4OH+ 
Aq.  (Fremy,  A.  ch.  (3)  23.  407.) 

SI.  sol.  in  H2O.  Very  si.  sol.  in  KOH  and 
K2C03+Aq.  Insol.  in  NH4OH+Aq.  Insol. 
in  HNO3+H2SO4.  Slowly  sol.  in  cold,  quickly 
in  hot  HCl+Aq.  SI.  sol.  in  tartaric  and 
oxalic  acid  and  in  KHC2O4 + Aq.  (Senderens, 
Bull.  Soc.  1899,  (3)  21.  48.) 

Insol.  in  acetone.  (Naumajm,  B.  1904,  37. 
4329.) 

Pf/roantimonic  acid,  H4Sb2O7. 

More  sol.  in  H2O  and  acids  than  H3SbO4. 
Sol.  in  cold  NH4OH,  or  KOH+Aq.  (Fremy.) 
Slowly  sol.  in  cold  H2O. 

5.88  g.  Sb2O5  in  1  1.  H2O  at  15° 
8.55  "      "      "  1  1.     "     "  25° 
21.30  "      "      "  1  1.     "     "  60° 
(Delacroix,  J.  Pharm.  1897,  6.  337-41.) 


40 


ANTIMONIC  ACID 


SI.  sol.  in  H2O.  Very  si.  sol.  in  KOH  and 
K2CO3+Aq.  Insol.  in  NH4OH+Aq,  and  in 
HNO3+H2SO4.  Slowly  sol.  in  cold,  quickly 
in  hot  HCl+Aq.  SI.  sol.  in  tartaric  acid, 
oxalic  acid  and  KHC2O4+Aq.  (Senderens, 
Bull.  Soc.  1899,  (3)  21.  48.) 

Or^oantimonic  acid,  H3Sb04. 

SI.  sol.  in  H2O.  Insol.  in  NH4OH+Aq. 
Easily  sol.  in  KOH+Aq.  (Fremy.) 

Does  not  exist.    (Raschig,  B.  18.  2745.) 

Has,  however,  been  prepared  by  Daubrawa 
(A.  186.  110),  Conrad  (C.  N.  40.  198),  and 
Beilstein  and  Blaese  (Bull.  Ac.  St.  Petersb. 
33.  97). 

Very  sol.  in  H2O.  (Delacroix,  Bull  Soc. 
1899  (3)  21.  1049.) 

Very  si.  sol.  in  H20,  in  KOH  and  K2CO3  + 
Aq.  Slowly  sol.  in  cold,  quickly  in  hot  HC1  + 
Aq.  Insol.  in  NH4OH+Aq,  and  in  HN03  + 
H2SO4.  SI.  sol.  in  tartaric  acid,  oxalic  acid 
and  KHC2O4+Aq.  (Senderens,  Bull.  Soc. 
1899,  (3)  21.  52.) 

+  HH2O.    (Beilstein  and  Blaese.) 

According  to  Beilstein  and  Blaese  only  one 
antimonic  acid,  H3SbO4,  exists. 

TWrantimonic  acid,  Sb2O5+4H20=H8Sb2O9. 

Slowly  sol.  in  cold  H20. 

Solution  sat.  at  t°  contains  g.  Sb2O5  per 
litre  — 

t°  15°  25°  60°          70° 

g.  Sb206     5.88     8.3-8.75      21.30      53.89 

Decomp.  in  solution  by  heating  to  100°  or 
long  standing  in  the  cold  to  Sb2O5,  3H2O. 
(Delacroix,  Bull.  Soc.  1899,  (3)  21.  1049.) 

Insol.  in  H2O.  Very  si.  sol.  in  KOH  and 
K2CO3+Aq.  Slowly  sol.  in  cold,  quickly  in 
hot  HCl+Aq.  Insol.  in  NH4OH+Aq.  Insol. 
in  HNO3+H2SO4.  SI.  sol.  in  tartaric  acid, 
oxalic  acid  and  in  KHC2O4  +  Aq.  (Senderens, 
Bull.  Soc.  1899,  (3)  21.  51.) 

#ezantimonic  acid,  Sb2O5+6H2O  = 


Sol.  in  H2O  to  the  extent  of  22  g.  Sb2O6  per  1. 
but  on  standing  becomes  turbid  and  a  white 
powder  is  pptd.  until  finally  only  3  g.  Sb2O5 
are  dissolved  per  1.  (Senderens,  Bull.  Soc. 
1899,  (3)  21.  48-49.) 

Antimonates. 

a.  Antimonates.  From  HSbO3.  Some  of 
the  K  and  NH4  salts  are  sol.  in  H2O,  the  others 
are  slightly  sol.  or  insol. 

ft.  Pyroantimonates.  From  H4Sb2O7.  As 
a  class,  insol.  in  H2O,  but  decomp.  thereby  ex- 
cept in  presence  of  large  excess  of  alkali 
(Fremy,  A.  ch.  (3)  12.  499.) 

Probably  do  not  exist.  (Beilstein  and 
Blaese.) 

Aluminum  antimonate,  A12O3,  3Sb2O5  (?). 

Ppt.  Somewhat  sol.  in  excess  of  Al  salts 
+Aq.  Insol.  in  K4Sb2O7+Aq. 

Al(Sb03)3+15H20  =  AlH6(Sb0 


Ppt.  (Beilstein  and  Blaese,  Bull.  Ac.  St. 
Petersb.  33.  101.) 

Al(SbO3)3  +  7H2O  =  AlH6(SbO4)3  +  4H2O. 
Ppt.  (B.  and  B.) 

A12O3,  Sb2O5+9H2O.  Ppt.  (Ebel,  B.  22. 
3043.) 

Ammonium    antimonate,    NH4SbO3+2H2O, 

Insol.  in  H2O. 

+2^H20.  Insol.  in  HoO.  (Senderens, 
Bull.  Soc.  1899,  (3)  21.  56.) 

+6H20.    See  (NH4)2H2Sb2O7+5H2O. 

Ammonium  pyroantimonate,  (NH4)4Sb2O7. 

Known  only  in  solution. 

(NH4)2H2Sb2O7+5H2O. 

Sol.  in  H2O,  but  decomp.  by  standing  or 
boiling  into  insol.  salt.  Insol.  in  alcohol. 
(Fremy,  J.  pr.  45.  215).  Composition  is 
NH4SbO3+6H2O,  according  to  Raschig  (B. 
18.  2743). 

Barium  antimonate,  Ba(SbO3)2. 

Ppt.  Scarcely  sol.  in  H2O.  Slowly  sol.  in 
BaCl2+Aq. 

+2H2G.  Somewhat  sol.  in  H2O.  Easily 
sol.  in  HCl+Aq.  (Delacroix,  Bull.  Soc. 
1899,  (3)  21.  1051.) 

+5,  or  6H2O.    Ppt. 

BaSb4O7+5H2O.  Sol.  in  cone.  HC1.  (Dela- 
croix, Bull.  Soc.  1899,  (3)  21.  1051.) 

BaO,  3Sb2O5+5H2O.  Insol.  in  H2O.  In- 
completely sol.  in  HC1.  (Delacroix,  I.e.) 

BaO,  4SboO5+15H2O.    (Delacroix,  I.e.) 

9BaO,  10Sb205  +  18H2O.  Insol.  in  HC1  + 
Aq.  (Delacroix,  I.e.) 

Bismuth  antimonate,  BiSbO4+H2O. 

Ppt.  Insol.  in  H2O;  sol.  in  HCl+Aq. 
(Cavazzi,  Gazz.  ch.  it.  15.  37.) 

3Bi2O3,  Sb2O6+H2O.  Insol.  in  H2O;  sol. 
in  HCl+Aq.  (Cavazzi.) 

2Bi2O3,  Sb2O5.    As  above.    (Cavazzi.) 

Cadmium  antimonate,  Cd(SbO3)2+2H2O. 

Insol.  in  H2O.  (Senderens,  Bull.  Soc.  1899. 
(3)  21.  56.) 

+3HH2O.  Very  sol.  in  H2O.  Sol.  in  HC1 
+Aq.  (Ebel,  Dissert.  1890.) 

+5H2O.    Insol.  in  H2O.    (Senderens,  I.e.) 

+6H2O.  Ppt.  Insol.  in  H20.  (Ebel,  B. 
22.  3043.) 

Calcium  antimonate,  Ca(SbO3)2. 

Ppt. 

+5H2O.    Ppt.    (Heffter,  Pogg.  86.  418.) 

+6H2O.  Insol.  in  H2O.  (Senderens,  Bull. 
Soc.  1899,  (3)  21.  56.) 

3CaO,  2Sb2O6+6H2O.    Min.  Ullmanite. 

Chromic  antimonate,  Cr(SbO3)3+14H2O. 
Ppt.    (Beilstein  and  Blaese.) 

Cobaltous  antimonate,  Co(SbO3)2+5H2O. 

Insol.  in  H2O.  Loses  3H2O  in  the  presence 
of  H2SO4  and  passes  into  Co(SbO3)2+2H2O, 


ANTIMONATE,  POTASSIUM 


41 


also  insol.  in  H2O.      (Senderens,  Bull.  Soc. 

1899,  (3)  21.  55.) 

+6H2O.    Ppt.    (Ebel,  B.  22.  3043.) 
+7H2O.    SI.  sol.  in  H2O.    SI.  sol.  in  boiling 

solutions  of  cobalt  salts. 

+  12H2O.    Ppt.    (Heffter,  Pogg.  86.  448.) 

Cobaltous  hydrogen  antimonate,  CoH4(SbO4)2 

+H20. 
(Gorgeul,  Ann.  Phys.  Beibl.  1897,  21.  198.) 

Cupric  antimonate,  3CuO,  2Sb2O6. 

Ppt.    (Beilstein  and  Blaese.) 

Cu(SbO3)2.  Insol.  in  H2O,  acids,  or  alkalies. 
(Berzelius.) 

+2H2O.  Insol.  in  H20.  (Senderens,  Bull. 
Soc.  1899,  (3)  21.  55.) 

+5H2O.    Ppt.    (Ebel,  B.  22.  3043.) 

Insol.  in  HoO.    (Senderens,  I.e.) 

CuO,  2Sb2O6+9H2O.  Insol.  in  H2O.  Sol. 
in  Sb2O6,  4H2O+Aq.  (Delacroix,  Bull.  Soc. 
1899,  (3)  21.  1054.) 

2CuC,  3Sb2O5  +  10H2O.  Insol.  in  H2O. 
Sol.  in  NH4OH  and  in  fn'antimonic  acid-f-Aq. 
(Delacroix,  I.  c. 

CuO,  6Sb2O5  +  16H2O.    (Delacroix,  I.e.) 

Cupric    antimonate     ammonia,     Cu(SbO3)2, 
4NH3+4H2O. 

Insol.  in  HoO  and  NH4OH+Aq.  (Schiff, 
A.  123.  39.) 

CuSb2N3H21O12  =  Cu(ONH4)OH, 
2(NH4SbO3+2H20).    (Raschig,  B.  18.  2743.) 

Cu(SbO3)o,3NH3+9H2O.  (Delacroix,  BuU. 
Soc.  1901,  (3)  25.  289.) 

Glucinum  antimonate,  Gl(Sb03)2+6H2O. 

Somewhat  sol.  in  hot  H2O.  Easily  sol.  in 
warm  HC1.  (Ebel,  Dissert.  1890.) 

Iron  (ferrous)  antimonate. 
SI.  sol.  in  H2O.    (Berzelius.) 

Iron  (ferric)  antimonate. 

Insol.  in  H2O.    (B.) 

Fe2O8,  Sb2O5+7H2O.  Ppt.  (Ebel,  B.  22 
3043.) 

Fe2O3,  2Sb2O5  +  llH2O.  Ppt.  (Beilstein 
and  Blaese.) 

Fe(SbO3)3+6^H2O.    Ppt.    (B.  and  B.) 

Lead  antimonate,  basic,  Pb3(SbO3)2(OH)4+ 
Pb3(SbO4)2+4H2O. 


Min.    Bleinerite,  Bindheimite. 
2Pb(SbO3)2,  PbO  +  llH2O.    Ppt.    (B.  and 
B.) 

Lead  antimonate,  Pb(SbO3)2. 

Insol.  in  H2O.     Incompletely  decomp.  bj 

acids.    (Berzelius.) 
Naples  Yellow.    Insol.  in  H2O. 
+2H2O.    Insol.  in  H2O.    (Senderens,  Bull 

Soc.  1899,  (3)  21.  57.) 

+5H20.    Ppt.     (Ebel,  B.  22.  3043.) 
+6H2O.    Ppt.    (Beilstein  and  Blaese.) 
+9H2O.    Insol.  in  H2O.    (Senderens,  I.e.) 


Lead  antimonate  chloride,  Pb(SbO3)2,  PbCl2. 
Min.  Nadorite.    Sol.  in  HC1,  HNO3,  and 
tartaric  acid+Aq. 

Lithium  antimonate,  LiSbO3. 

SI.  sol.  in  cold,  sol.  in  hot  H20,  and  crys- 
tallizes on  cooling.  Much  more  sol.  than 
NaSb03. 

+3H2O.  Ppt.  SI.  sol.  in  H2O.  (Beilstein 
and  Blaese.) 

Magnesium  antimonate,  Mg(SbO3)2  +  12H2O. 
Sol.  in  hot,  less  sol.  in  cold  H2O.  (Heffter.) 
Sol.  in  MgSO4+Aq;  insol.  in  KSbO3+Aq. 

(Berzelius.) 

Manganous  antimonate,  Mn(SbO3)2. 
Difficultly  sol.  in  H2O. 
When  heated,  is  sol.  only  in  strong  acids. 
+2H2O.    Insol.  in  H2O.    (Senderens,  Bull. 

Soc.  1899,  (3)  21.  56.) 

+5H2O.    Ppt.    (Ebel,  B.  22.  3043.) 
+6H2O.    Insol.  in  H2O.    (Senderens,  I.e.) 
-j-7H2O.    Ppt.    (Beilstein  and  Blaese.) 

Mercurous  antimonate. 
Insol.  in  H2O.    (Berzelius.) 

Mercuric  antimonate,  Hg(SbO3)2. 

Insol.  in  H2O,  alkalies,  and  most  acids. 

SI.  attacked  by  boiling  H2SO4,  and  HC1+ 
Aq. 

+2H2O.  Insol.  in  H,O.  (Senderens,  Bull. 
Soc.  1899,  (3)  21.  55.) 

+5H-.O.    Insol.  in  H2O.    (Senderens.) 

+6H2O.    Ppt.    (Beilstein  and  Blaese.) 

Nickel  antimonate,  Ni(SbO3)2+2H2O. 

Insol.  in  H2O.  (Senderens,  Bull.  Soc.  1899, 
(3)  21.  54.) 

+5H2O.    Insol.  in  H2O.    (Senderens.) 

+6H2O.  Ppt.  Insol.  in  H2O.  (Heffter, 
Pogg.  86.  446.) 

+  12H2O.    SI.  sol.  in  H2O.    (Heffter.) 

Potassium  antimonate,  KSbO3. 

Insol.  in  H2O.  Sol.  in  warm  KOH+Aq,  but 
separates  nearly  completely  on  cooling.  By 
boiling  with  H2O,  or  by  standing  for  a  long 
time  with  cold  H2O,  it  gradually  dissolves  as 
2KSbO3+5H2O,  or  K2H2Sb2O7+4H2O,  or 
2KH2SbO4+3H2O. 

Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.  257.) 

+H2O.  Insol.  in  H2O.  (Senderens,  Bull. 
Soc.  1899,  (3)  21.  57.) 

+1^H2O  (=2KSbO3+5H2O  of  Fremy). 
Easily  sol.  in  H2O,  especially  if  warm.  Solu- 
tion is  pptd.  by  NH4Cl+Aq.  (Fremy,  A. 
ch.  (3)  12.  499.) 

+2^H2O.  100  pts.  H2O  at  20°  dissolve 
2.81  pts.  anhydrous  salt;  sp.  gr.  of  solution 
sat.  at  18°  =  1.0263.  Composition  is  given  as 
K2H2Sb2O7 +4H2O.  (Knorre  and  Olschewsky, 
B.  20.  3043.) 

.    Insol.  in  H2O.    (Senderens,  I.e.) 


42 


ANTIMONATE,  POTASSIUM 


+4^H2O.  Sol.  in  H2O.  (Delacroix,  J 
Pharm.  1897,  (6)  6.  533.) 

2KoO,  3Sb2O5+10H2O.  SI.  sol.  in  H2O 
(Delacroix,  J.  Pharm. -1897,  6.  337.) 

+  10H2O.    (Delacroix,  I.e.) 

Potassium  pT/roantimonate,  K4Sb2O7. 

Deliquescent;  decomp.  by  boiling  with  H20 
into  KSb03+5H2O,  by  cold  H2O  into 
K2H2Sb2O7+6H2O.  (Fremy.) 

Does  not  exist.    (Knorre  and  Olschewsky.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1904,37.3601.) 

Potassium  hydrogen  pf/roantimonate, 
K2H2Sb2O7. 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014.) 

+2^H2O.  (Senderens,  Bull.  Soc.  1899,  (3) 
21.  57.) 

+3HH2O.  Very  difficultly  sol.  in  hot  or 
cold  H2O.  (Knorre  and  Olschewsky,  B.  18. 
2358.) 

+6H2O.  Quite  difficultly  sol.  in  cold  H2O. 
Not  precipitated  by  NH4Cl+Aq.  Aqueous 
solution  gradually  decomposes.  (Fremy.) 

+4H2O.    See  2KSbO3+5H2O. 

Potassium      antimonate      sulphantimonate, 

KSbO3,  K3SbS4+5H2O. 
Decomp.  on  air,  and  with 'cold  H2O.    Sol. 
in  hot  H2O.    (Rammelsberg.) 

Silver  antimonate. 

Insol.  in  H2O.    (Berzelius.) 

AgSbO3+3H2O=AgH2SbO4+2H2O.  Eas- 
ily sol.  in  NH4OH+Aq,  when  freshly  pptd. 
(Beilstein  and  Blaese.) 

+1>^H2O.    Ppt.    (Ebel,  B.  22.  3043.) 

Silver     antimonate     ammonia,     AgH2SbO4, 

2NH3+H20. 
(Beilstein  and  Blaese.) 

Sodium  antimonate,  NaSbO3. 

Sol.  in  much  H2O,  but  soon  becomes  de- 
composed into  Na2H2Sb2O7. 

+3HH2O,  composition  of  Na2H2Sb207+ 
6H2O,  according  to  Beilstein  and  Blaese. 

1000  pts.  H2O  dissolve  0.31  pt.  NaSbO3+ 
3HH2O  at  12.3°. 

1000  pts.  alcohol  of  15.8%  dissolve  0.13  pt. 
NaSbO3+3^H2O  at  12.3°. 

1000  pts.  alcohol  of  25.6%  dissolve  0.07  pt 
NaSb03+3KH20  at  12.3°. 

Somewhat  more  sol.  when  freshly  precipi- 
tated. 

Absolutely  insol.  in  glacial  HC2H3O2. 

Presence  of  NaOH  or  Na  salts  diminish  sol- 
ubility, while  NH4OH  or  K  salts  increase  it 


slightly.    (Beilstein  and  Blaese,  Bull.  Ac.  St. 

Petersb.  33.  201.) 

+4^H2O.    Sol.  inH20.     (Delacroix,  Bull. 

Soc.  1899,  (3)  21.  1051.) 

2Na2O,  3Sb2O5+10H2O.    (Delacroix,  I.  c.) 
Na2O,  3Sb2O6+HH2O.     (Delacroix,  L  c.) 

Sodium      pvroantimonate,      Na2H2Sb2O7  + 

6H20. 

Boiling  H2O  dissolves  yj^  pt.  of  this  salt. 
(Fremy.)  1000  pts.  H2O  dissolve  2.5  pts.  salt. 
(Ebel,  B.  22.  3044.)  See  also  NaSbO3+ 


+5H20.    (Knorre  and  Olschewsky.) 

Strontium  antimonate,  Sr(Sb03)2+6H20. 

Ppt.  Less  sol.  in  H2O  than  SrS04.  (Heff- 
ter,  Pogg.  86.  418.) 

Thallous  antimonate,  TlSbO3+2HoO  = 

TlH2SbO4+H2O. 

Somewhat  sol.  in  H2O,  when  freshly  precipi- 
tated; insol.  when  dried.  (Beilstein  and 
Blaese.) 

Tin  (stannous)  antimonate,  2SnO,  Sb2O5. 

Ppt.    (Lenssen,  A.  114.  113.) 

Sn(SbO3)2  +2H2O.  Attacked  with  difficulty 
by  acids  or  alkalies,  most  easily  by  hot  cone. 
H2SO4.  (Schiff,  A.  120.  55.) 

2SnO,  3Sb2O5+4H2O. 

SnO,  2Sb2O5. 

Tin  (stannic)  antimonate. 

Insol.  in  H2O.    (Levol,  A.  ch.  (3)  1.  504.) 

Uranium  antimonate,  5U02,  3Sb2O5+15H2O. 
Ppt.  Sol.  in  hot  cone.  HCl+Aq,  and  in 
UCl3+Aq.  (Rammelsberg.) 

Zinc  antimonate,  Zn(SbO3)2. 

Very  slightly  sol.  in  H2O  (Berzelius);  sol. 
in  solutions  of  Zn  salts. 

+2H2O.    (Ebel,  Dissert.  1890.) 

Insol.  in  H2O.  (Senderens,  Bull.  Soc.  1899, 
(3)  21.  57.) 

+5H2O.  Not  wholly  insol.  in  cold,  mod- 
erately sol.  in  hot  H2O.  (Ebel,  Dissert.  1890.) 

+6H2O.    Insol.  in  H2O.    (Senderens.) 

Antimoniomolybdic  acid. 

Ammonium  antimoniomolybdate,  5(NH4)2O, 

4Sb2O5,  7MoO3  +  12H2O. 
Readily  sol.  in  hot  H2O.    (Gibbs,  Am.  Ch. 
J.  7.  392.) 

Antimoniotungstic  acid,  3Sb2O6,  4W03+ 

11H2O. 

Sol.  in  H2O.  (Hallopeau,  C.  R.  1896,  123. 
1068.) 

Potassium  antimoniotungstate,  3K20.  3Sb2O5, 

4W03+4H20. 

Much  more  sol.  in  hot  than  in  cold  H2O. 
Decomp.  by  HC1,  H2SO4  and  HNO3.  (Hallo- 
peau, C.  R.  1896,  123.  1066.) 


ANTIMONY 


43 


+  16H2O.  Much  more  easily  sol.  in  ho 
than  cold  H2O.  Decomp.  by  HC1,  H2SO 
and  HNO3.  (Hallopeau,  I.e.) 

6K2O,  4Sb2O5,  12WO3+25H2O. 

SI.  sol.  in  H2O.    (Gibbs,  Am.  Ch.  J.  7.  392 

Antimoniuretted  hydrogen. 
See  Antimony  hydride. 

Antimonosomolybdic  acid. 

Ammonium  antimonosomolybdate,  6(NH4)2C 

3Sb2O3,  17MoC3+21H2O. 
Insol.  in  cold  H2O.    (Gibbs,  Am.  Ch.  J.  7 
313.) 

Antimonosophosphotungstic  acid. 

Potassium  antimonosophosphotungstate, 

12K2O,  5Sb2O3,  6P2O5,  22W03+48H2O. 
Nearly  insol.  in  cold  or  warm  H2O.    (Gibbs 
Am.  Ch.  J.  7.  392.) 

Antimonosotungstic  acid. 

Ammonium  antimonosotungstate. 
Sol.  in  H2O. 

Barium  antimonosotungstate,  4BaO,  6Sb2O3 

22W03+36H20. 

Precipitate;  very  si.  sol.  in  hot  H»O.  (Gibbs 
Am.  Ch.  J.  7.  313.) 

Antimonous  acid,  HSbO2. 

(Long,  J.  Am.  Chem.  Soc.  1895,  17.  87.) 
+1^H20.    Ppt.    (Schaffner,  A.  51.  182.) 
H3SbO3.    Ppt.     (Clarke  and  Stallo,  B.  13. 

1793.) 

Does  not  exist.    (Guntz,  C.  R.  102.  1472.) 
H4Sb2O6.    When  freshly  pptd.,  is  sol.  in  dil 

KOH,    and    NaOH+Aq.      Scarcely   sol.    in 

NH4OH+Aq,  or  in  (NH4)2CO3,  or  KHCO3+ 

Aq. 

Completely  sol.  in  K2CO3,  and  Na2CO3+ 

Aq,  especially  if  warm.    When  recently  pptd. 

is  si.  sol.  in  succinic  acid+Aq. 

Calcium  antimonite,  CaSb2O4  (?). 

Min.  Romeite.    Insol.  in  acids. 
Cobaltous  antimonite  (?). 

SI.  sol.  in  H2O.    (Berzelius.) 
Cuprous  antimonite,  Cu6(SbO3)2. 

Insol.  in  H2O.  Sol.  in  acids;  most  easily  in 
cone.  HCl+Aq.  (Hausmann  and  Stromeyer, 
Schw.  J.  19.  241.) 

Cupric  antimonite  (?). 

Insol.  in  H2O.    (Berzelius.) 

CuSb2O5.    Min.  Ammiolite. 

CuSb2O4.  Sol.  in  HCl+Aq,  tartaric  and 
citric  acids.  (Harding,  Z.  anorg.  1899,  20. 

Iron  (ferrous)  antimonite  (?). 

More  sol.  in  H2O  than  the  antimonate. 

(Dumas.) 


Potassium  antimonite,  K2O,  3Sb2O3. 

Easily  decomp.  by  cold  H20.  Not  decomp 
by  KOH+Aq  containing  over  20.9%  K2O. 
(Corimimbceuf,  C.  R.  115.  1305.) 

+3H2O.    As  above.    (C.) 

Potassium  antimonite  iodide,  K2O,  8Sb2O3, 
2KI. 

Insol.  and  not  decomp.  by  cold  or  hot  H2O. 
Not  decomp.  by  acids  or  alkalies.  Aqua  regia 
decomp.  slowly.  Tartaric  acid  dissolves 
gradually.  (Griihl,  Dissert.  1897.) 

Sodium  antimonite,  NaSbO2+3H2O. 

Difficultly  sol.  in  H2O.  (Terreil,  A.  ch.  (4) 
7.  380.) 

2Na2O,  3Sb2O3+H2O.  Decomp.  by  H2O, 
but  not  by  NaOH+Aq  containing  94.3  g. 
NaOH  per  1.  (Corimimbceuf.) 

Na2O,  2Sb2O3.  Decomp.  by  H2O  but  not 
by  NaOH+Aq  containing  188.6  g.  NaOH 
per  1.  (C.) 

Na20,  3Sb2O3.  Decomp.  by  H2O,  but  not 
by  NaOH+Aq  containing  113.2  g.  NaOH 
per  1.  (C.) 

+2H20  =  NaH2(Sb02)3.    (Terreil.) 

Antimony,  Sb. 

Does  not  decomp.  H2O.  Not  attacked  by 
HCl+Aq  (Berzelius);  slowly  sol.  in  cone.  HC1 
+Aq  (Debray) ;  slowly  sol.  in  cone,  warm  HC1 
+Aq  (Troost).  Attacked  by  very  cone.  HC1 
+Aq  only  when  finely  divided  (Schutzen- 
berger,  Willm);  very  si.  attacked  by  dil.  or 
cone,  acid  (Guntz).  Not  attacked  by  boiling 
HCl+Aq  (Gmelin).  By  careful  experiments, 
pure  Sb  is  absolutely  insol.  in  dil.  or  cone.,  hot 
>r  cold  HCl+Aq,  except  when  in  contact  with 
>xygen.  (Ditte  and  Metzner,  A.  ch.  (6)  29. 
889.) 

Insol.  in  dil.  or  cold  cone.,  but  sol.  in  hot 
one.  H2SO4.    Oxidized  but  not  dissolved  by 
HNO3+Aq.     Easily  and  completely  sol.  in 
aqua  regia. 

Very  slowly  attacked  by  pure  HNO3+Aq  of 

51-1.42  sp.  gr.;  weaker  acid  has  no  marked 

action  whether  it  contains  NO  2  or  not .   HC1 + 

HNO3  has  no  action  if  dil.  or  at  low  temp.,  but 

vhen  even  very  dil.  and  KNO2  is  added,  the 

ction  will  begin.    (Millon,  A.  ch.  (3)  6.  101.) 

Not  attacked  in  10  months  by  2%  HNOs 
+Aq.    Sb  is  not  dissolved  by  HNO3+Aq  of 
ny  concentration,  a  white  powder  being  al- 
ways left,  which  is  insol.  in  HNO3+Aq  or 
T2O.    (Montemartini,  Gazz.  ch.  it.  22.  384.) 

Insol.  in  alkalies +Aq. 

Somewhat  sol.  in  distilled  H2O.    More  or 
ess  sol.  in  solutions  of  acids,  alkalies  and  salts 
nd  in  alcohol  and  ether.    Only  si.  sol.  in  a 
mixture  of  alcohol  and  ether.    (Ruff  and  Al- 
ert, B.  1905,  38.  54.) 

Alkaline  H2O2  converts  Sb  into  antimonic 
cid,  but  neutral  H2O2  is  without  action. 
Hark,  Chem.  Soc.  1893,  63.  886.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
898,  20.  826.) 


44 


ANTIMONY  ARSENIDE 


Easily  attacked  by  pyrosul; 
(Heumann  and  Kochlin,  B.  li 
Sb  is  sol.  in  a  mixture  of  HIS 
acid  or  other  polybasic  acids 
anal.  1906,  45.  507.) 
Not  attacked  by  a  mixture 
ether.    (Cohen,  Z.  phys.  Ch. 
1A  cc.  oleic  acid  dissolves 
6  days.     (Gates,  J.  phys.  Ch 
There  are  three  modificatio 
1.  Ordinary  gray  metallic. 
2.  Black   amorphous.      Ur 
temp.     By  boiling  with  H2C 
metallic  Sb. 
3.  Yellow.     Very  unstable, 
over  rapidly  into  the  ordinary 
tion.     Sol.  in  CS2  at  a  littl 
(Stock,  B.  1903,  37.  898.) 
Unstable  above  —90°.    (St< 
3837.) 

Antimony  arsenide,  Sb2As. 
(Descamps,  C.  R.  86.  1065 

Antimony  ^n'bromide,  SbBr3. 
Deliquescent;  decomp.  by 
Very  sol.  in  liquid  NH3. 
J.  1898,  20.  826.) 
Very  sol.  in  warm  liquid  ^ 
solution  with  sp.  gr.  =  3.685  a 
Z.  phys.  Ch.  1893,  11.  339.) 
Sol.  in  S2C12.    (Walden,  Z. 
217.) 
Sol.  in  AlBr3.     (Isbekow, 
64.  27.) 
Easily  sol.  in  PC13  and  PB 
anorg.  1900,  25.  211.) 
Sol.  in  alcohol  and  CS2. 
Sol.  in  ether  forming  two  la^ 
Chem.  Soc.  1902,  24.  360.) 
Sol.  in  acetone.     (Naumai 
4328.) 

Solubility  of  SbBr3  in  org 
Data  in  parentheses  indicat 
rium. 

3hurvl  chloride. 
J.  479.) 
rO3  and  tartaric 
(Czerwek,  Z. 

of  alcohol  and 
1904,  47.  12.) 
[).0007  g.  Sb  in 
1911,  15.  143.) 
ns. 

istable   at   ord. 
>  is  changed  to 

Solubility  of  SbBr3  in  organic  liquids.  —  Cont. 

Solvent 

t°    - 

jj8 

S" 

^^ 

t° 

j38 

01-1 

sa 

t° 

jig 

h. 

lod- 
benzene 

—28.6° 
—30.5 
—32 
—20 
—10 
0 

0 
4.0 
8.7 
13.5 
17.5 
21.7 

10° 
20 
30 
40 
50 
60 

26.3 
31,5 
37.3 
43.7 
50.7 
58.5 

70° 
80 
90 
94 

67.0 
78.2 
91.9 
100 

68.9 
85.2 
100 

Paradi- 
chlor- 
benzene 

54.5° 
51.5 
48.5 
55 

0 
6.3 
12.8 
18.7 

65° 
70 
75 
80 

29.5 
37.0 
45.6 
56.2 

85° 
90 
94 

At  —  50°  goes 
black  modifica- 
e  above  —90°. 

3ck,  B.  1905,  38. 

) 

H2O. 

;Gore,  Am.  Ch. 

.sBr3,  forming  a 
b47°.    (Retgers, 

anorg.  1900,  26. 
Z.  anorg.  1913, 
r3.    (Walden,  Z. 

^ers.    (Hayes,  J. 
in,  B.  1904,  37. 

anic  liquids, 
e  labile  equilib- 

Paradi- 
brom- 
benzene 

88° 
85 
80 
75 
70 

'0 

6.8 
18.0 
29.5 
41.5 

65° 
70 
75 
80 
85 

52.0 
59.1 
66.5 
74.4 
83.0 

90° 
92 
94 

91.8 
95.4 
100 

Nitro- 
benzene 

6° 
1 

,    A 

—  9 
—15 
(—17) 

0 
8.6 
17.0 
24.0 
29.7 
(31.9) 

—5° 
5 
15 
25 
35 
45 

32.3 
35.3 
38.8 
42.8 
47.4 
52.8 

49.1 
53.0 
54.4 
56.1 
58.8 
62.2 
66.2 

55° 
65 
75 

85 
90 
94 

59.1 
66.4 
74.9 
86.0 
93.0 
100 

70.8 
76.0 
81.7 
87.8 
94.2 
100 

Metadi- 
nitro- 
benzene 

90° 
85 
80 
75 
70 
65 
60 

0 
8.1 
16.2 
24.2 
31.8 
38.5 
44.3 

55° 
50 
47.5 
50 
55 
60 
65 

70° 
75 
80 
85 
90 
94 

Toluene 

—93° 
—93.5 
—70 
—50 
—30 
—10 
—  1 

0 
0.3 
1.2 
2.6 
5.2 
13.3 
22.4 

10° 
20 
30 
(34) 
40 
50 
60 

28.8 
36.7 
47.5 
(54.0) 
51.5 
56.3 
62.3 

70° 
80 
85 
90 
94 

69.4 
79.4 
85.2 
92.6 
100 

59.8 
67.4 
77.4 
85 
92.6 
100 

Ethyl- 
benzene 

—93° 
—60 
—40 
—20 
—10 
0 

0.1 
0.4 
1.0 
2.3 
3.9 
6.4 

0.4 
1.2 
3.4 
5.5 
9.5 
17.2 
24.3 

10° 
20 
25 
29 
40 
50 

9.8 
19.5 
28.6 
37.8 
44.6 
51.6 

60° 
70 
80 
85 
90 
94 

Propyl- 
benzene 

—80° 
—60 
—40 
—30 
—20 

(—1.5°) 
(-20, 

10 
20 
30 
40 

(33.3) 
(23.3) 
25.8 
27.8 
30.5 
34.1 
38.6 

50° 
60 
70 
80 
90 
94 

44.3 
51.5 
61.5 
73.5 
90 
100 

35.8 
43.3 
54.0 
68.5 
90 
100 

Solvent 

t° 

f. 

^    FH 

%& 

t° 

* 

sl 

t 

!§ 
a& 

—  5 

Isoamyl- 
benzene 

—70° 
—50 
—40 
—30 
—20 
—17 
(—15) 

1.9 
3.6 
5.1 
7.1 
13.4 
16.4 
(19.4) 

(—13°) 
—10 
0 
10 
20 
30 
40 

(24.9) 
17 
18.2 
19.9 
22.5 
25.9 
30.3 

50° 
60 
70 
80 
90 
94 

Benzene 

5.6° 
4.5 
15 
25 
35 
45 
55 

0 
1.9 
3.0 
4.3 
6.0 
8.6 
12.1 

0 
1.7 
2.2 
3.2 
4.3 
5.6 

0 
2.6 
4.4 
6.9 
9.9 
13.4 

65° 
75 
80 
85 
90 
91.5 
92.5 

0° 
10 
20 
30 
40 
50 

17.1 
24.9 
30.7 
38.4 
48.2 
58.1 
66.6 

91.5° 
90 
85 
90 
92 
94 

73.7 
76.7 
84.9 
91.4 
94.8 
100 

(Menschutkin,  Ann.  Inst.  Pol.  P.  le  Gr.  13.  1.) 

Antimony  bromide  with  MBr. 
See  Bromantimonate,  M. 
Also  below. 

Antimony  hydrogen  bromide,  SbBr5,  HBr+ 
3H2O. 

Very    hygroscopic.      Decomp.    by    H2O 
(Weinland  and  Feige,  B.  1903,  36.  256.) 
See  Metabromantimonic  acid. 

Chlor- 
benzene 

-^5.2° 
—47 
—40 
—30 
—20 
—10 

7.2 
9.2 
11.8 
15.4 
20.8 
28.1 

60° 
70 
80 
90 
94 

37.6 
50.0 
66.6 
89.6 
100 

Brom- 
benzene 

—31° 
—32 
—25 
—1.5 

5 

15° 
25 
35 
45 
55 
65 

17.4 
22.2 
22.7 
34.4 
42.6 
52.6 

75° 
85 
90 
94 

65.2 
81.1 
90.0 
100 

ANTIMONY  CHLORIDE 


45 


Antimony  caesium  bromide.  2SbBr6,  3CsBr+ 
2H20. 
Loses  Bro  in  the  air.    (Weinland,  B.  1903, 
36.  257.) 

Antimony  calcium  bromide,  SbBr3,  CaBr2+ 
8H2O. 
Easily    decomp.      (Benedict,    Proc.    Am. 
Acad.  1895,  30.  9.) 

Antimony  glucinum  bromide,  3SbBr5,  2GlBr2 
+  18H20. 
Hydroscopic.    Easily  decomp.    (Weinland, 
B.  1903,  36.  258.) 

Solubility  in  H2O. 
100  pts.  SbCl3  sol.  in  pts.  H20  at  t°. 

t° 

Pts.  H2O 

0° 
15° 
20° 
»    25° 
30° 
35° 
40° 
50° 
60° 

16.6 
12.3 
10.9 
10.1 
9.4 
8.7  • 
7.3 
5.2 
2.2 

f\/InrvvV*v,-»tr      V       r.-n^T./v       1  OAQ       O9      OOft    'V 

Antimony  magnesium  bromide,  SbBr3)  MgBr2 

+8H2O. 

As  Ca  salt.  (Benedict,  Proc.  Am.  Acad. 
1895,  30.  9.) 

Antimony     potassium     bromide,     10SbBr3, 

23KBr+27H20. 
(Herty,  Am.  Ch.  J.  1894,  16.  496.) 

Antimony  rubidium  bromide,  2SbBr3,  3RbBr. 

Decomp.  by  H2O;  can  be  recryst.  from  dil. 
HBr+Aq.  (Wheeler,  Z.  anorg.  5.  258.) 

SbRb2Br6.  Slowly  loses  Br2  in  the  air. 
Decomp.  by  H2O.  (Weinland,  B.  1903,  36. 
259.) 

10SbBr3,  23RbBr  (?).  Cryst.  from  cone. 
HBr+Aq.  (Wheeler.) 

The  composition  assigned  to  this  salt  by 
Wheeler  (Z.  anorg.  5.  253)  is  incorrect. 
(Ephraim,  B.  1903,  36.  1817.) 

Antimony  vanadium  bromide,  SbBr3,  VBr4+ 

7H2O. 

Hydroscopic.  Decomp.  by  H20.  Sol.  in 
dil.  HC1  and  in  tartaric  acid.  (Weinland,  B. 
1903,  36.  260.) 

Antimony  bromide  potassium  chloride,  SbBr3, 


Solubility  in  HCl+Aq. 

100  mol.  H2O  dissolve  mol.  SbCl3  in  presence 

of  mol.  HC1  at  20°. 


e  po 

20. 


Slowly  deliquescent.    Very  sol.  in  H20. 

Sat.  solution  contains  120.5  g.  to  100  cc. 
H2O,  and  has  sp.  gr.  =  1.9. 

Decomp.  by  much  H20.  (Atkinson,  Chem. 
Soc.  43.  200.) 

Does  not  exist.  (Herty,  Am.  Ch.  J.  1894, 
16.  497.) 

See  also  Antimony  chloride  potassium 
bromide. 

Antimony  bromofluoride,  SbF6Br. 

Decomp.  by  H2O.  (Ruff,  B.  1906,  39. 
4319.) 

Antimony  trichloride,  SbCl3. 

Deliquescent.  Decomp.  by  H2O  with  pre- 
cipitation of  SbOCl.  This  precipitation  is  pre- 
vented by  tartaric,  citric,  or  hydrochloric  acid, 
or  by  cone,  solutions  of  chlorides  of  alkalies 
and  alkaline  earths. 


Mol.  HC1 

Mol.  SbCls 

0 

72.1-72.8 

2.4 

73.0 

6.5 

67.5 

8.4 

67.6 

8.6 

66.5 

9.8 

65.0 

12.2 

65.3 

29.6 

54.5 

(Meerburg,  Z.  anorg.  1903,  33.  304.) 

Solubility  in  HCl+Aq. 

100  mol.  H2O  dissolve  at  20° 

Solid  phase 

1 

2 

3 

4 

Mol. 

Mol. 

Mol. 

Mol. 

SbCls 

HC1 

SbOCl 

HC1 

SbOCl 

8.7 

7.2 

9.8 

6.9 

8.6 

7  5 

16.1 

7.9 

19.6 

8.0 

21.7 

7.4 

19.8 

8.9 

25.0 

8.8 

28.0 

8.6 

(SbOCl)x,(SbCl3)y 

37.5 

8.7 

32.0 

7.9 

44.0 

6.8 

35.8 

7.9 

63.7 

6.2 

59.5 

6.4 

69.1 

5.6 

61.0 

6.5 

66.1 

4.6 

62.7 

4.4 

69.8 

5.3 

SbCl3  and 

69.3 

4.3 

(SbOCl)x,(SbCl8)y 

68.3 

3.6 

1  &  2.  (Meerburg,  Z.  anorg.  1903,  33.  302.) 
3  &  4.     (Noodt,  Z.  anorg.  1903,  33.  302.) 

Somewhat  sol.  in  liquid  (CN)2.  (Cent- 
nerszwer,  Bull.  Soc.  1901,  (3)  28.  405.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  826.) 

Easily  sol.  in  PC13  and  PBrs.  (Walden,  Z. 
anorg.  1900,  26.  211.) 

Sol.  in  S2ri2.  (Walden,  Z.  anorg.  1900,  25. 
217.) 


46 


ANTIMONY  CHLORIDE 


Easily  sol.  in  AsBr3.     (Walden,  Z.  anorg 
1902,  29.  374.) 
Sol.  in  afcohol  without  decomp.    Very  sol 
in  hot  CS2,  but  solubility  diminishes  rapidly 
on  cooling.     (Cooke.   Proc.  Am.  Acad.  13 
72.) 
1  g.  SbCls  is  sol.  in  0.186  g.  acetone  at  18° 
Sp.  gr.  of  sat.  solution  18°/4°  =  2.216..  (Nau- 
mann,  B.  1904,  37.  4332.) 
Sol.  in  ethyl  acetate.    (Naumann.  B.  1904, 
37.  3601.) 
1  pt.  sol.  in  16.97  pts.  of  ethyl  acetate  at 
18°.     Sp.  gr.  of  sat.  solution  18°/4°  =  1.7968. 
(Naumann,  B.  1910,  43.  320.) 
Sol.  in  benzonitrile.     (Naumann,  B.  1914, 
47.  1369.) 
Sol.  in  methylal.     (Eidmann,  C.  C.  1899, 
II.  1014.) 

Solubility  of  SbCl3  .in  organic  liquids. 
Data  in  parentheses  indicate  labile  equilib- 
rium. 

Solubility  of  SbCl3  in  organic  liquids  —  Cont. 

Solvent 

t° 

|l 

s| 

t° 

o 

n 

t° 

o 

j»2 
3* 

<£? 

68.8 
73.2 
78.5 
85.8 
_95.2 
100 

59.3 
66.6 
71.1 
77.1 
83.8 
94.7 
100 

Metadi 
nitro- 
benzene 

90° 
80 
70 
60 
40 
(20) 
(1) 
(—11) 

0 
14.3 
25.3 
33.8 
45.6 
(53.6) 
(59.  S) 
(62.2) 

(—10°) 
(10) 
(27.5) 
(28.5) 
27.5 
25 
(20) 
(10) 

(57.7 
(.62.4 
(44.5 
(50.0 
55.0 
60.2 
(66.2 
(73.5 

(0°) 
20 
30 
40 
50 
60 
70 
73 

Toluene 

—93° 
—94 
—70 
—50 
—40 
—30 
—20 

0 
0.5 
1.4 
3.3 
5.1 
7.2 
10 

—10° 
0 
6 
11 
(—8) 
20 
30 

14.4 
22.1 
28.6 
35.7 
(27.0) 
40.5 
47.6 

40° 
42.5 
40 
50 
60 
70 
73 

Ethyl- 
benzene 

—93° 
—50 
—30 
—10 
0 
10 
20 
30 

0.1 
u.6 
1.1 
3.6 
5.6 
9.4 
16.8 
27.2 

35° 
39 
37 
35 

(33) 
(15) 
(25) 
37 

36.4 
50 
57.7 

61.8 

(65.7) 
(37.8) 
(47.5) 
66.6 

(36.8)° 
(33) 
40 
50 
60 
65 
70 
73 

(68.1) 
(65.7) 
70.3 
77.3 
85.5 
90.3 
95.6 
100 

53.2 
53.6 
56.9 
60.6 
65.5 
72 
81 
86.8 
95.1 
100 

Solvent 

t° 

|i 

*l 

t° 

•o 
"o^ 

S| 

t° 

-1 

"o 

ss, 

Propyl- 
benzene 

(—70°) 
(—50) 
(—40) 
(—30) 
(—20) 
(—10) 
(—5) 
(0) 
(1.5) 
(1) 

(0.6) 
(2.8) 
(5.2) 
(8.8) 
14.8) 
25.1) 
32.4) 
43.3) 
(50) 
51.1) 

—70° 
—50 
—  40 
—30 
—20 
—10 
—5 
0 
5 
7 

0.2 
1.5 
3.0 
5.5 
9.7 
16.2 
20.5 
26.2 
35.6 
41.6 

8.5° 
10 
20 
30 
40 
50 
60 
65 
70 
73 

Benzene 

5.6° 
4 
1 

,      10 
1      20 
30 
40 

0 
2.6 
7.1 
10.1 
13.1 
16.8 
21.4 

50° 
60 
70 
75 

77.5 
79 
77.5 

27.2 
34.7 
45.2 
53.1 
58.7 
66.6 
73.4 

75° 
70 
62 
67.5 
73 

78.5 
83.3 
89.3 
94.2 
100 

Chlor- 
benzene 

—  45.2° 

—40 
—30 
—20 
—15 

0 
2.2 
3.6 
6.0 
9.0 
11.6 

J14.4 
19.4 
28.1 
(41  .  1) 
32.5 
38.7 

30° 
40 
50 
60 
70 
73 

47.1 
56.2 
66.6 
78.7 
94.3 
100 

—5 
0 
(4) 
10 
20 

Iso- 

amyl- 
oenzene 

—80° 
—70 
—  60 
—50 
—  40 
(—30) 
(—25) 
(—22) 
—20.5) 
(—22) 

3 
5.4 

8.4 
12.4 
17.9 

27.3) 
34.4) 
40.7) 
(50) 
(54) 

(—45°) 
(—35) 
—25 
—15 
—5 
(0) 
(5) 
(7.5) 
(—21) 
(—10) 

(17.1) 
(22  .  8) 
29.3 
36.6 
45.6 
52.3) 
60.3) 
66.6) 
44.2) 
44.9) 

0° 
10 
20 
30 
40 
50 
60 
65 
70 
73 

46.3 
48.8 
52.5 
57.3 
63.4 
71.4 
81.7 
88 
95.5 
100 

Brom- 
benzene 

lod- 
benzene 

—31° 
—32.5 

(—35) 
—30 

0 
3.4 

(6.4) 
4.8 
7.6 
10.7 
14.1 
17.8 

—5° 
0 
3 
(6) 
(7) 
10 
20 
30 

21.7 
26.6 
31.8 
41.9) 
50.0) 
36.4 
43.2 
50.8 

40° 
50 
60 
65 
70 
73 

59.2 
68.8 
80.6 
87.2 
95.0 
100 

53.9 
60.4 
67.5 
76.2 
87.4 
95.0 
00 

—20 
—15 
—10 

(Menschutkin,  Ann.  Inst.  Pol.  P.-le  Gr.,  13.  1.) 

Antimony  hydrogen  fnchloride,  2SbCl3,  HC1 
+2H20. 
Deliquescent.    Decomp.  by  H2O. 
Melts  in  crystal  H2O  at  16°.    (Engel,  C.  R. 
106.  1797.) 

Antimony  pentachloride,  SbCl5. 
Deliquesces  to  SbCl5+4H2O,  which  can  be 
crystallized  out  of  a  little  H20.    Decomp.  by 
more  H2O  into  SbO2Cl.    Sol.  in  a  large  amt. 
of  H2O,  if  it  is  added  all  at  one  time.    Precipi- 
;ation  by  H2O  is  also  hindered  by  presence  of 
tartaric,  or  hydrochloric  acid. 
+H2O.    Deliquescent.    Sol.  in  chloroform. 
(Anschiitz  and  Evans,  A.  239.  285.) 
+4H20.    Insol.  in  chloroform.    (Anschutz 
and  Evans.) 

Antimony  pentacbloride  with  MCI. 
See  Chlorantimonate,  M. 
See  also  below. 

—28.6° 
—30 

(—35) 
(—40) 
(—45) 
(—35) 
(—25) 
(—15) 

0 

2.4 
(11.7) 
(20.8) 
(27.2) 
(30.9) 
(33.9) 
(37.2) 

(—5)° 
—34.5 
—25 
—15 
—5 

<-?> 

15 

40.7) 
10.7 
16.4 
24.7 
39.1 
47.2) 
44.5 
48.7 

25° 
35 
45 
55 
65 
70 
73 

Paradi- 
chlor- 
benzene 

Paradi-; 
brom- 
benzene 

54.5° 
50 
45 
40 

0 
6.3 
15.5 

28.0 

39.5° 
45 
50 
55 

29.5 
37.5 
46.4 
56.0 

60° 
65 
70 
73 

66.5 
78.1 
91.1 
00 

88° 
85 
80 
75 
70 

0 
5.9 
15.8 
25.7 
35.7 

65° 
60 
49.5 
55 
60 

45.4 
53.8 
64.9 
72.5 
79.8 

65° 
70 
73 

87.1 
95.2 
00 

Nitro- 
benzene 

6° 
2 
—2 

—6 
—10 
—14 

(—18) 
—16.5 

0 

7.0 
12.1 
16.5 
20.3 
23.5 
26.2) 
25.2 

—13.5° 
—10.5 
—7.5 
—6.5 
—6 
—6.5 
—5 
5 

27.3 
29.8 
35.2 
40.7 
50.0 
52.8 
53.0 
55.8 

15° 
25 
35 
45 
55 
65 
70 
73 

59.2 
63.0 
67.6 
72.8 
79.0 
87.2 
92.7 
00 

ANTIMONY  POTASSIUM  CHLORIDE 


47 


Antimony    hydrogen     pentachloride.    SbCls, 


"  A/etachlorantimonic  acid"  according  to 
Weinland  and  Schmid,  (Z.  anorg.  1905,  44. 
43.) 

Very  easily  sol.  in  H20,  alcohol,  acetone 
and  glacial  acetic  acid.  Aqueous  solution 
decomp.  on  standing  with  separation  of  Sb2O5 
but  remains  clear  in  presence  of  10%  HC1. 
(Weinland  and  Schmid,  Z.  anorg.  1905,  44. 
43.) 

SbCl5,  5HC1+10H2O.  Not  deliquescent. 
Decomp.  by  H2O.  Melts  in  crystal  H20  at 
about  55°.  (Engel,  C.  R.  106.  1797.) 

Antimony  antimonyl  chloride,  SbCl3,  SbOCl. 
More  easily  attacked  by  H2O  than  SbOCl. 
(Bemmelen,  Z.  anorg.  1903,  33.  293.) 

Antimony  antimonyl  potassium  chloride. 
SbCl3,  SbOCl,  2KC1. 

Not  deliquescent.  Immediately  decomp.  by 
hot  or  cold  H2O;  sol.  in  hot  glacial  HC2H302, 
or  in  HC1,  or  tartaric  acid+Aq. 

Insol.  in  KCl+Aq,  hot  or  cold  alcohol,  CS2, 
or  ligroine.  (Benedikt,  Proc.  Am.  Acad.  29. 
217.) 

Antimony     antimonyl     rubidium     chloride, 

SbCl3,  SbOCl,  2RbCl. 
Sol.  in  very  dil.  HCl+Aq.  .  (Wells,  Am.  J. 
Sci.  1897,  (4)  3.  463.) 

Antimony  barium  chloride,  SbCl3,  BaCl2+ 

3/2H20. 
Decomp.  by  H2O. 

Antimony  caesium  chloride,  SbCl3,  GCsCl. 

Decomp.  by  H2O.  Cryst.  from  dil.  HC1+ 
Aq.  (Godeffroy,  Arch.  Pharm.  (3)  12.  47.) 

2SbCl3,  3CsCl.  Decomp.  by  H20;  si.  sol. 
in  cold,  easily  in  hot  dil.  HCl+Aq.  This  is 
identical  with  the  above  salt.  (Saunders,  Am. 
Ch.  J.  14.  152.) 

SbCl4,  2CsCl.  Sol.  in  boiling  cone.  HC1+ 
Aq  without  decomp.  (Setterberg,  Oef.  Vet. 
Akad.  1882,  6.  23.) 

SbCl6,  CsCl.  Cryst.  from  HC1  +  Aq  without 
decomp.  Decomp.  by  H2O.  (Setterberg, 
Oef.  Vet.  Akad.  1882,  6.  27.) 

Antimony  calcium  chloride,  SbCl3,  CaCl2+ 
8H2O. 

Easily  decomp.  (Benedict,  Proc.  Am. 
Acad.  1895,  30.  9.) 

SbCl6CaSbCl6.OH+9H20.  Deliquescent; 
si.  sol.  in  H2O.  (Weinland,  B.  1901,  34.  2635.) 

Antimony  chromium  chloride, 

CrCl3,  3SbCl5+13H2O.    (Weinland.) 
should  be 

[SbCl6]3[Cr(OH2)6]+7H2O; 
and  CrCl3,  SbCl5  +  10H2O  should  be 

[SbCl6][Cr(OH2)4Cl2]+6H2O. 

(Pfeiffer,  Z.  anorg.  1903,  36.  349.) 


Antimony  glucinum  chloride,  SbCl3,  G1C1-.+ 
3H20. 

Very  hydroscopic.  Decomp.  by  H2O. 
Very  easily  sol.  in  HC1.  (Ephraim,  B.  1903, 
36.  1822.) 

+4H,O.  Ppt.  Decomp.  by  H20.  Sol. 
in  HC1.  (Ephraim,  B.  1903,  36.  1822.) 

Antimony    hydrazine    chloride,    SbCl3, 

3N2H5C1. 

Sol.  in  cone.  HCl+Aq;  decomp.  by  H2O. 
(Ferratini,  C.  A.  1912,  1613.) 

Antimony  lithium  chloride,  SbCl3,  2LiCl+ 
5H2O. 

Hydroscopic.  Decomp.  by  H2O.  Very 
easily  sol.  in  HC1.  (Ephraim,  B.  1903,  36. 
1821.) 

+6H2O.  Decomp.  by  H2O;  easily  sol.  in 
HC1.  (Ephraim,  B.  1903,  36.  1822.) 

Antimony  magnesium  chloride,  SbCl3,  MgCl2 
+5H20. 

Hydroscopic.  Decomp.  by  H2O.  Can  be 
cryst.  from  HC1  without  decomp.  (Ephraim, 
B.  1903,  36.  1823.) 

2SbCl3,  MgCU-  Hygroscopic.  Decomp. 
by  H2O.  Very  sol.  in  HC1.  (Ephraim.) 

SbClrMeSbCleMgOH  +  17H2O.  Hydro- 
scopic. Sol.  in  H2O  with  decomp.  (Weinland, 
B.  1901,  34.  2635.) 

Antimony  nitrosyl  chloride,  SbCl5,  NOC1. 

Very  deliquescent;  decomp.  by  pure  H2O; 
sol.  in  H20  containing  tartaric  acid.  (Weber, 
Pogg.  123.  347.) 

2SbCl5,  5NOC1.  Decomp.  by  H2O.  (Sud- 
borough,  Chem.  Soc.  59.  661.) 

Antimony  phosphorus  chloride,  SbCl5,  PC15. 
Deliquescent.    (Weber,  Pogg.  125.  78.) 

Antimony  phosphoryl  chloride,  SbCl5,  POC13. 
Deliquescent.    (Weber.) 

Antimony  platinum  potassium  chloride, 

(Sb,  Pt)CUKi. 
Ppt.    (Weinland,  B.  1905,  38.  1086.) 

Antimony  potassium  chloride,  SbCl3,  2KC1. 

Sol  in  H2O  without  decomp.  (Jacquelain, 
A.  ch.  (2)  66.  128.) 

Not  deliquescent.  Immediately  decomp. 
by  hot  or  cold  H2O.  Sol.  in  HC1,  or  tartaric 
acid+Aq.  (Benedikt,  Proc.  Am.  Acad.  29. 
219.) 

+2H2O.    Very  efflorescent. 

SbCls,  3KC1.  "  Deliquescent.  Decomp.  by 
hotH20.  (Poggiale.)  _,-,-.., 

+2H2O.    (Romanis,  C.  N.  49.  273.) 

Not  obtained  by  Benedikt  (I.e.) 

10SbCl3,23KCl.  True  composition  of  above 
salts.  Sol.  inH2O.  (Herty,  Am.  Ch.  J.  1894, 
16.  495.) 

SbCl3,  2KC1  is  the  only  true  compound,  all 


48 


ANTIMONY  RUBIDIUM  CHLORIDE 


others  being  isomorphous  mixtures.  (Jordis, 
B.  1903,  36.  2539.) 

2SbCl4,  3KC1.  Deliquescent.  Decomp.  by 
H2O.  (Bosek,  Chem.  Soc.  1895,  67.  516.) 

SbCtebCleKOH.  Hydroscopic.  Sol.  in 
H2O  with  decomp.  (Weinland,  B.  1901,  34. 
2635.) 

See  also  Antimony  antimonyl  potassium 
chloride. 

Antimony  rubidium  chloride,  SbCl3,  RbCl. 

Decomp.  on  air  or  with  H20.  (Saunders, 
Am.  Ch.  J.  14.  162.) 

2SbCl3,RbCl+H2O.  Decomp.  on  air. 
(Wheeler,  Z.  anorg.  5.  253.) 

SbCl3,  6RbCl.  Decomp.  by  H2O.  (Godef- 
froy,  Arch.  Pharm.  (3)  9.  343.) 

Formula  is  10SbCl3,  23RbCl  (?).  (Saunders 
Am.  Ch.  J.  14.  159.) 

10SbCl3,  23RbCl  (?).  Decomp.  by  H2O; 
sol.  in  HCl-fAq.  (Saunders.) 

Formula  is  3SbCl8,7RbCl.  (Wells  and 
Foote,  Am.  J.  Sci.  1897,  (4)  3.  461.) 

Composition  assigned  to  this  salt  by 
Saunders  (Am.  Ch.  J.  14.  155)  is  incorrect. 
(Ephraim,  B.  1903,  36.  1817.) 

3SbCl3,  5RbCl.    As  above.    (Saunders.) 

Formula  is  2SbCl3,  3RbCl.    (Wheeler.) 

Rb2SbCl6.  Ppt.  Decomp.  by  H2O.  (Wein- 
land, B.  1905,  38.  1083.) 

Rb2SbCl6,  2Rb3SbCl6.  Ppt.  Decomp.  by 
H2O.  (Weinland,  B,  1901,  34.  2635.) 

Antimony  selenium  chloride,  SbCl5,  SeCl4. 
Deliquescent.    (Weber.) 

Antimony  selenyl  chloride,  SbCl6,  SeOCl2. 

Very  deliquescent.  (Weber,  Pogg.  125. 
325.) 

Antimony  sodium  chloride,  SbCl3,  3NaCl  (?). 
Decomp.  by  much  H20.    (Poggiale.) 

Antimony  sulphur  chloride,  2SbCl5,  3SC12. 

Decomp.  by  H2O. 

SbCl6,  SC14.    Sol.  in  dil.  HN03+Aq. 

Mpt.  125-126°  in  an  atmos.  of  chlorine. 
Violently  decomp.  by  H20.  (Ruff,  B.  1904, 
37.  4515.) 

Antimony  thallium  chloride,  SbCl3,  3T1C1. 
Ppt.    (Ephraim,  Z.  anorg.  1909,  61.  249.) 
SbCl4,  T1C1.      (Ephraim  and   Barteczko, 

Z.  anorg.  1909,  61.  251.) 

2SbCl4,  2T1C1,  T1C13.    Slowly  decomp.  by 

cold    H2O.      (Ephraim    and    Barteczko,    Z. 

anorg.  1909,  61.  253.) 

Antimony  trichloride  ammonia,  SbCl3,  NH3. 
Not  very  deliquescent.    Decomp.  by  H2O. 

Antimony     pentochloride    ammonia,    SbCl5, 

6NH3. 
Decomp.  by  H2O.    (Persoz.) 


Antimony     pewfachloride    cyanhydric    acid, 

SbCl5,  3HCN. 

Deliquescent;  decomp.  by  H20.  (Klein,  A. 
74.  85.) 

Antimony  pewtachloride  nitric  oxide,  2SbCl6, 

NO. 

Decomp.  by  H2O.  (Besson,  C.  R.  108. 
1012.) 

Antimony   pewtochloride   nitrogen   peroxide, 

3SbCl5,  2NO2. 
Decomp.  by  H2O.    (Besson.) 

Antimony  pentachloride   nitrogen   sulphide, 

SbCl5,  N4S4. 

Easily  decomp.  (Davis,  Chem.  Soc.  1906, 
89.  1577.) 

Decomp.  by  cold  H2p,  HC1,  H2SO4  and 
warm  alcohol,  also  by  boiling  with  KOH+Aq. 
Almost  insol.  in  organic  solvents.  (Wolbling, 
Z.  anorg.  1908,  57.  283.) 

Antimony  chloride  potassium  bromide, 
SbCl3,3KBr+lHH2O. 

Very  deliquescent.  Decomp.  by  much 
H2O.  (Atkinson,  Chem.  Soc.  43.  289.) 

2SbCl3,3KBr+2H2O.    (Atkinson.) 

SbCl3,KBr+H20.    (Atkinson.) 

Above  are  mixtures.  (Herty,  Am.  Ch.  J. 
1894,  16.  497.) 

See  Antimony  bromide  potassium  chloride. 

Antimony  chlorofluoride,  SbCl3F2. 
(Swarts,  Z.  anorg.  1896,  12.  71.) 

Antimony  fluoiodide,  SbF6I. 

Slowly  decomp.  by  H2O.  (Ruff,  B.  1906, 
39.  4321.) 

(SbF5)2I.  Sol.  in  H2O  with  pptn.  of  I2. 
(Ruff,  B.  1906,  39.  4321.) 

Antimony  Znfluoride,  SbF3. 
Deliquescent.    Sol.  in  H2O. 

Solubilitv  in  H2O  at  t°. 


t° 

100  g.  of  the 
solution  con- 
tain g.  SbF3 

100  g.  H2O 
contain  g.  SbFs 

0° 
20 
22.5 
25 
30 

79. 

81. 
81. 
83. 

84. 

37 
64 
91 
12 
93 

384.7 
444.7 
452.8 
492.4 
563.6 

(Rosenh'eim,  Z.  anorg.  1909,  61.  189.) 
Solubility  in  HF+Aq  at  0°. 

Normality  of  HF+Aq 

100  g.  H2O  of  the  HF  solu- 
tion dissolve  g.  SbFs 

2 
1 
0.5 

474.9 
432.5 
404.0 

(Rosenheim,  Z.  anorg.  1909,  61.  192.) 

ANTIMONY  FLUORIDE  POTASSIUM  CHLORIDE 


49 


Solubility  of  SbF3  in  salts  +Aq  at  0°. 

Antimony  lithium  fluoride,  SbF3,  2LiF.  ' 
Sol.  in  more  than  20  pts.  H2O.    (Fliickinger, 
Pogg.  87.  245.) 
SbF3,  LiF.     Easily  sol.  in  H20.    "(Stein, 
Chem.  Z.  13.  357.) 

Antimony  potassium  fluoride,  SbF8,  2KF. 
Sol.  in  less  than  2  pts.  boiling,  and  in  9  pts. 
cold  H2O.    Insol.  in  alcohol  or  ether. 
SbF3,KF.   More  sol.  than  SbF3,  2KF.   Sol. 
in  2.8  pts.  H2O.    (Fliickinger,  Pogg.  87.  245.) 
SbF6,  KF.    Easily  sol.  in  H2O. 
SbF6,  2KF+2H2O.     Easily  sol.  in  H2O. 
(Marignac,  A.  146.  239.) 

Antimony  sodium  fluoride,  SbF3,  3NaF. 
Sol.  in  14  pts.  cold,  and  4  pts.  boiling  H2O. 
Sol.  in  HF.    (Fliickinger,  Pogg.  87.  245.) 
SbF3,  NaF.     100  pts.  cold  H2O  dissolve  93 
pts.     100  pts.   hot  H2O   dissolve    166   pts. 
(Stein,  Wagners'  J.  B.  1887.  1160.) 
4SbF3,  NaF.     As  NH4  salt.     (Raad  and 
Hauser,  B.  1890,  23.  R.  125.) 
SbF6,  2NaF.    Easily  sol.  in  H2O.    (Marig- 
nac, A.  145.  329.) 

Antimony  thallium  fluoride,  TlF,SbF3. 
Sol.  in  H20  without  decomp.     (Ephraim, 
B.  1909,  42.  4458.) 
TlF,2SbF3.    Sol.  in  H2O  without  decomp. 
(Ephraim.) 
TlF,3SbF8.    Sol.  in  H2O  without  decomp. 
Decomp.  by  cold  cone.  H2SO4.     (Ephraim.) 

Antimony  Znfluoride  ammonia,  SbF3,  2NH8. 
SI.  sol.  in  liquid  NH3.    (Ruff,  B.  1906,  39. 
4326.) 

Salt 

Normality  of 
salt  solution 

100  g.  H2O  of  the 
salt   solution   dis- 
solve g.  SbF8 

KC1 

1 

0.5 
0.25 
0.125 

461.8 
448.3 
431.9 
407.3 

KBr 

1 
0.5 
0.25 
0.125 

448.7 
450.0 
455.6 
417.2 

KNOi 

1 
0.5 
0.25 
0.125 

458.2 
451.9 
418.3 
401.4 

^K2S04 

1 
0.5 
0.25 

419.9 
408.5 
406.6 

^K2C204 

1 
0.5 
0.25 
0.125 

465.7 
481.2 
451.3 
405.2 

K(NH4)2C204 

0.5 
0.25 
0.125 

431.9 
442  3 
433.3 

HK2C4H406 

1 
0.5 
0.25 
0.125 

461.4 
430.5 
430.8 
435.2 

(Rosenheim,  Z.  anorg.  1909,  61.  192.) 

Insol.  in  liquid  NH3.     (Gore,  Am.  Ch.  J. 
1898,  20.  826.) 

Antimony  pentafluoride,  SbF6. 

Sol.  in  H2O.    (Marignac,  A.  146.  239.) 
Very  hydroscopic;  bpt.  155°.    Sol.  in  H2O 

with  hissing.    (Ruff,  B.  1904,  37.  678.) 
+2H2O.    (Ruff,  B.  1904,  37.  679.) 

Antimony     pentafluoride      diantimony     trir 

fluoride,  Sb3Fn=2SbF3,  SbF5. 
Hydroscopic;  bpt.  390°.    Easily  sol.  in  H2O. 
(Ruff,  B.  1904,  37.  680.) 

Antimony    pentofluoride   penfoantimony   iri- 

fluoride,  SbF6,  5SbF3. 
B  pt.  384°  (corr.).    (Ruff,  B.  1904,  37. 681.) 

Antimony  caesium  fluoride, 

CsF,2SbF3. 

CsF,3SbF3. 
4CsF,7SbF3. 

CsF,SbF3. 
2CsF,SbF3. 
(Wells,  Am.  J.  Sci.  1901,  (4)  11.  451.) 


Antimony    Znfluoride    ammonium    chloride. 

SbF3,  NH4C1. 
Easily  sol.  in  H2O.    (de  Haen,  B.  21.  901 

R.) 

Antimony   /nfluoride   ammonium    sulphate, 

SbF3,  (NH4)2S04. 

More  sol.  than  K  or  Na  salt.  1  pt.  H2O 
dissolves  1.4  pts.  at  24°  and  15  pts.  at  100°. 
(de  Haen,  B.  21.  902  R.) 

Antimony  fluoride   lithium   chloride,   SbFj, 

LiCl. 
Sol.  in  H2O.    (Stein,  Chem.  Z.  13.  357.) 

Antimony     pewtafluoride    nitrosyl    fluoride, 

SbF5,  NOF. 

Hydroscopic.  Decomp.  by  H20.  Sol.  in 
liquid  NH3  with  decomp.  SI.  sol.  in  NOC1, 
SiCl4,  PC13,  AsCl3,  SO2C12  and  SOC12.  (Ruff, 
Z.  anorg.  1908,  68.  334.) 

Antimony    influoride    potassium    chloride, 

SbF3,  KC1. 

100  pts.  H2O  dissolve  51  pts.  at  24°,  and 
300  pts.  at  100°.  (de  Haen,  B.  21.  901  R.) 


50 


ANTIMONY  FLUORIDE  POTASSIUM  SULPHATE 


Antimony    Znfluoride    potassium    sulphat 
SbF3,  K2S04. 

Sol.  in  H2O.    (de  Haen.) 

2SbF3,  K2S04.    Very  sol.  in  H,0.    (Mayer 
B.  1894,  27.  R.  922.) 

Antimony  fnfluoride  sodium  chloride,  SbF; 

NaCl. 
Easily  sol.  in  H2O.    (de  Haen,  B.  21.  90 

Antimony  influoride  sodium  sulphate,  SbF3 

Na2S04. 
Sol.-inH20.    (deHaen.) 

Antimony  fluoiodide,  SbF5I. 

Mpt.  80°;  slowly  decomp.  by  H20.  (Ruff 
B.  1906,  39.  4321.) 

(SbF6)2I.      Mpt.    110-115°:    decomp. 
H2O.    (Ruff.) 

Antimony  fluosulphide,  SbF5S. 

Very  hygroscopic.  Decomp.  by  H2O.  Sol 
with  decomp.  in  alcohol.  Sol.inCCl4.  (Ruff 
B.  1906,  39.  4332.) 

Antimony  gold,  Au3Sb. 

Insol.  in  equal  pts.  of  HN03  and  tartaric 
acids.  (Roessler,  Z.  anorg.  1895,  9.  72.) 

Antimony  hydride,  SbH3. 

Scarcely  sol.  in  H2O.  1000  ccm.  H2O  ab- 
sorb 4.12  cc.  SbH3  at  10.5°.  Decomp.  by 
long  contact  with  H2O;  also  by  cone.  H2SO4 
or  KOH+Aq.  (Jones,  Chem.  Soc.  29.  641.) 

Antimony  ZnTiydroxide,  SboO3,  2H2O  = 

Sb2O(OH)4. 
(Schaffner,  A.  51.  182.) 
Sb(OH)3.    Ppt.    (Clarke  and  Stolla,  B.  13. 

Does  not  exist.    (Guntz,  C.  R.  102.  1472.) 
See  Antimonous  acid  and  antimony   tri- 
oxide. 

Antimony  ^niodide,  SbI3. 

Decomp.  by  H2O  or  80%  alcohol.  Sol.  in 
HI+Aq;  sol.  in  boiling  CS2,  and  in  boiling 
benzene,  but  separates  out  on  cooling.  Al- 
most insol.  in  CHC13.  (Cooke,  Proc.  Am. 
Acad.  (2)  5.  72.) 

Easily  sol.  in  AsBr3.  (Walden,  Z.  anorg. 
1902,  29.  374.) 

Sol.  in  warm  AsBr3.  Sp.  gr.  of  a  solution 
sat.  at  40°,  which  solidifies  at  37°,  =3.720. 
This  dissolves  further  AsI3,  whereby  the  mpt. 
sinks  to  31°  and  sp.  gr.  rises  to  3.801.  By 
mixing  the  latter  solution  with  a  solution  of 
AsI3  in  CH2I2,  a  liquid  can  be  obtained  with 
a  sp.  gr.  of  3.702  at  20°.  (Retgers,  Z.  phys. 
Ch.  1893,  11.  340.) 

Sol.  in  PC13.  (Beckmann,  Z.  anorg.  1906, 
51.  110.) 

Sol.  in  SO2C12.     (Walden,  Z.  anorg.  1900, 


Sol.  in  SOC12  and  S2C12.  (Walden,  Z.  anorg. 
1900,  25.  216.) 

Sol.  in  AsCl3.  (Walden,  Z.  anorg.  1900, 
25.  214.) 

Sol.  in  SnCl4.  (Walden,  Z.  anorg.  1900, 
25.  218.) 

Sol.  in  POC13.  (Walden,  Z.  anorg.  1900, 
25.  212.) 

Easily  sol.  in  PC13  and  PBr3.  (Walden, 
Z.  anorg.  1900,  25.  211.) 

Partly  sol.  in,  and  partly  decomp.  by  al- 
cohol or  ether.  (M'lvor,  Chem.  Soc.  (2)  14, 
328.) 

Insol.  in  oil  of  turpentine  and  CC14. 

100  pts.  methylene  iodide  dissolve  11.3  pts. 
SbI3  at  12°;  sp.  gr.  of  solution  =  3.453.  (Ret- 
gers, Z.  anorg.  3.  343.) 

Sol.  in  C6H6.  (Retgers,  Z.  phys.  Ch.  1893, 
11.  334.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

Antimony  penfaiodide,  SbI5. 

Very  unstable.    (Pendleton,  C.  N.  48.  97.) 

Antimony  barium  iodide,  SbI3,  BaI2+9H2O. 
Decomp.  by  H2O.  Sol.  in  HC1,  HC2H302, 
or  H2C4H4O6+Aq.  CS2  dissolves  out  SbI3. 
(Schaffer,  Pogg.  109.  611.) 

Antimony  caesium  iodide,  2SbI3,3CsI. 

SI.  sol.  in  HI+Aq.  Exists  in  two  distinct 
brms.  (Wells,  Am.  J.  Sci.  1901,  (4)  11.  455.) 

Antimony   potassium  iodide,   2SbI3,   3KI  + 

3H2O. 

Decomp.  by  H2O.  Sol.  in  HC1,  HC2H3O2, 
or  H2C4H4O6+Aq.  CS2  dissolves  out  SbI3. 
Schaffer,  Pogg.  109.  611.) 

SbI3,  2KI+2MH2O.  Decomp.  by  H2O. 
Nickles,  J.  Pharm.  (3)  39.  116.) 

Antimony  rubidium  iodide,  2SbI3,  3RbI. 

Decomp.  by  H2O.  (Wheeler,  Z.  anorg.  5. 
59.) 

Antimony    sodium    iodide,    2SbI3,    3NaI  + 

12H2O. 
As  2SbI3,  3KI.    (Schaffer,  Pogg.  109.  611.) 

Antimony  thallous  iodide,  2SbI3,  3T1I. 

Decomp.  by  H2O  and  by  HCl+Aq,  also  by 
Icohol.  (Ephraim,  Z.  anorg.  1908,  58.  354.) 

Antimony  nitride,  SbN. 

Decomp.  by  heat.  (Franz  Fischer,  B.  1910, 
3.  1471.) 

Vntimony  irioxide,  Sb2O3. 

Very  si.  sol.  in  H2O.  Sol.  in  8900-10,000 
ts.  H2O  at  100°;  55,000-61,100  pts.  at  15°. 
Schulze,  J.  pr.  (2)  27.  320.) 

Sol.  in  HCl+Aq.  Insol.  in  HNO3+Aq,  but 
ot  as  insol.  as  metastannic  acid.  Sol.  in  cold 
uming  HNO8  or  H2SO4.  Insol.  in  dil.,  but 
ol.  in  cone,  alkalies,  or  alkali  carbonates + 


ANTIMONY  SULPHIDE 


51 


Aq.  Sol.  in  cold  NH4C1,  or  NH4NO3+Aq. 
Sol.  in  15  pts.  boiling  SbCl3.  (Schneider, 
Pogg.  108.  407.) 

Sol.  in  HC2H3O2,  or  HjCJ^O.+Aq,  and 
not  pptd.  from  these  solutions  by  H2O.  Eas- 
ily sol.  in  benzoic  acid.  Insol.  in  pyrotartaric 
acid.  Very  sol.  in  KHC4H4O6+Aq.  Sol.  in 
glycerine. 

Somewhat  sol.  in  H3PO4+Aq.  (Kohler, 
Dingl.  1885,  268.  520.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  826.) 

Sol.  in  lactic  acid.  (Kretzschmar,  Ch.  Z. 
1888,  12.  943.) 

Sol.  in  grape  sugar  solution  to  which 
Ca(OH)2  has  been  added.  (Vogel,  B.  1885, 
18,  R.  38.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Sol.  in  glycerine  in  presence  of  alkalies. 
(Kohler,  Dingl.  1885,  258.  520.) 

Exists  in  a  sol.  colloidal  modification. 
(Spring,  B.  16.  1142.) 

Min.  Valentinite,  Senarmontite. 

+H2O.    See  Antimonous  acid. 

Antimony  feiroxide,  Sb2O4. 

Insol.  in  H2O.  Slightly  attacked  by  acids; 
hot  cone.  HCl+Aq  acts  only  slightly.  ,(Fre- 
senius.) 

Min.  Cenantite.    SI.  sol.  in  HCl+Aq. 

Antimony  peroxide,  Sb2O5. 

Insol.  in  H2O.  Easily  sol.  in  HCl+Aq.  SI. 
sol.  in  cone.  KOH+Aq. 

"  Antimonoxyd"  is  sol.  in  glycerine  in  pres- 
ence of  alkalies. 

100  g.  glycerine,  to  which  have  been  added 
10  g.  NaOH+Aq  (1  :  1),  dissolve  20.6  g. 
at  b.-pt.;  20  g.  NaOH+Aq  (1  :  1),  dissolve 
36.0  g.  at  b.-pt.;  40  g.  NaOH+Aq  (1  : 1), 
dissolve  68.5  g.  at  b.-pt.;  80  g.  NaOH+Aq 
(1:1),  dissolve  93.0  g.  at  b.-pt.;  120  g.  NaOH 
+Aq  (1  :  1),  dissolve  119.2  g.  at  b.-pt. 
(Kohler,  Dingl.  258.  520.) 

See  also  Antimonic  acid. 

Antimony  nitrogen  pentoxide,  2Sb2O5,  N2O5. 
Not  decomp.  by  H2O.     (Thomas,  C.  R. 
1895,  120.  1116.) 

Antimony  oxybromide. 
See  Antimonyl  bromide. 

Antimony  oxy chloride. 
See  Antimonyl  chloride. 

Antimony  oxyfluoride. 
See  Antimonyl  fluoride. 

Antimony  oxysulphide,  Sb2OS2. 

Min.    Antimony  blende  (kermesite) . 

Insol.  in  H2O  or  dil.  acids,  except  HCl+Aq. 
(Schneider,  Pogg.  110.  147.) 


Antimony  palladium,  Sb2Pd. 

SI.  sol.  in  equal  pts.  of  HNO3  and  tartaric 
acids.  (Roessler,  Z.  anorg.  1895,  9.  69.) 

Antimony  platinum,  Sb2Pt. 

Insol.  in  equal  pts.  of  HNO3  and  tartaric 
acids.  (Roessler,  Z.  anorg.  1895,  9.  67.) 

Antimony  phosphide,  SbP. 

Insol.  in  benzene,  ether,  or  CS2.  (M'lvor, 
B.  6.  1362.) 

Antimony  selenide,  SbSe. 

(Chretien,  C.  R.  1906,  142.  1341.) 

Sb3Se4.    (Chretien,  I.e.) 

Sb4Se5.    (Chretien,  I.e.) 

Sb2Se3.  Sol.  in  KOH+Aq.  (Hof acker,  A. 
107.  6.) 

Sb2Se6.    (Hofacker.) 

Antimony  selenide,  with  M  selenide. 
See  Selenoantimonates,  M. 

Antimony  Znsulphide,  Sb2S3  (Kermes). 

Insol.  in  H2O  and  dil.  acids. 

1  1.  H2O  dissolves  5.2  x  10-6  mols.  pptd. 
Sb2S3  at  18°.  (Weigel,  Z.  phys.  Ch.  1907,  58. 
294.) 

Decomp.  by  cone.  HNO3  or  H2SO4.  Sol. 
in  cone.  HCl+Aq.  Easily  sol.  in  dil.  KOH, 
NaOH,  (NH4)2S,  and  K2S+Aq.  SI.  sol.  in 
NH4OH+Aq;  very  si.  sol.  in  (NH4)2CO3+ 
Aq;  insol.  in  KSH+Aq.  (Fresenius.) 

Sol.  in  a  mixture  of  50  pts.  H2O  and  18  pts. 
HC1  (sp.  gr.  1.16)  even  when  completely  sat. 
with  H2S.  (Lang  and  Carson,  J.  Soc.  Chem. 
Ind.  1902,  21.  1018.) 

SI.  sol.  in  H2SO3+Aq.  (Guerout,  C.  R. 
1872,  75.  1276.) 

Cryst.  Sb2S3  is  only  si.  sol.  in  NH4OH+ 
Aq  (1  pt.  in  about  2000  pts.  NH3). 

Pptd.  amorphous  Sb2S3  is  appreciably  more 
sol.  (1  pt.  in  600  pts.  NH3).  (Garot,  J.  pr. 
1843,  29.  83.) 

SI.  sol.  in  hot  2%  Na2B4O7+Aq,  still  less 
sol.  in  cold.  (Materne,  C.  C.  1906,  II.  557.) 

Insol.  in  NH4Cl+Aq. 

Sol.  in  14-15  pts.  pure  SbCl3.  -  (Schneider, 
Pogg.  108.  407.) 

Slowly  sol.  in  H2C4H4O6+Aq. 

Sol.  in  boiling' Na3SbS4+Aq. 

Sol.  in  hot  citric,  tartaric  and  oxalic  acids. 
SI.  sol.  in  malic,  benzoic,  picric  and  pyrogallic 
acids.  Insol.  in  formic  and  acetic  acids.  Es- 
pecially easily  sol.  in  citric  and  oxalic  acids 
with  addition  of  KNO3,  KNO2  or  KC1O3. 
(Bolton,  C.  N.  1878,  37.  86  and  99.) 

Sol.  in  ethylamine  sulphydrate+Aq. 

Min  Stibnite.  Sol.  in  cold  citric  acid+ 
Aq.  (Bolton,  C.  N.  37.  14.) 

Soluble  modification.  Sb2S3  may  be  ob- 
tained in  a  colloidal  state  in  aqueous  solution 
containing  1  pt.  Sb2S3  to  200  pts.  H2O.  This 
can  be  boiled  without  decomp.,  but  Sb2S3  is 
pptd.  by  acids  and  salts. 


52 


ANTIMONY  SULPHIDE 


Table  of  maximum  dilution  of  solutions  of 

Antimony  sulphur  dioxide,  SbSO2. 

acids  and  salts  which  cause  pptn.  of  Sb2S3. 

Ppt.    (Faktor,  C.  C.  1900,  I.  12J1.) 

HC1       .                         .     1  :  270 

H2S04  . 

. 

:  140 

Antimony  telluride,  SbTe. 

H2C204 

. 

:45 

Insol.  in  H2O. 

K2SO4   . 

(NH4)2S04 

• 

:65 
:130 

Sb2Te3.     Insol.  in  H2O.     (Oppenheim,  J. 
pr.  71.  277.) 

MgS04  . 

:  1720 

MnSO4  . 

:2060 

Antimonyl  bromide,  SbOBr. 

NaCl     . 
BaCl2    . 

• 

:  135 
:2050 

Insol.  in  CS2.    (Cooke,  Proc.  Am.  Acad.  13. 
104.  ^ 

MgCl2  . 
CoCl2    . 

:    : 

:5800 
L  :2500 

J.vr±./ 

SI.  sol.  in  liquid  NH3.    (Gore,  Am.  Ch.  J. 
1898,  20.  826.) 

KNO3   . 

Fe2Cl6   . 

Ba(N03)2 

.     1  :  id 
.     1  :  2500 
.     1  :  1250 

Sb405Br2.    (M'lvor,  C.  N.  29.  179.) 
10Sb4O5Br2,  SbBr3. 

K2A12(SO4)4 

1  :  35,000 

Antimonyl  chloride. 

(NH4)2Fe2(SO4)4   .         .     1  :  800 
K2Cr2(SO4)4  .         .         .     1  :  40,000 
KSbOC4H4Ofl         .        .     1  :  18 

From  SbCl3.   SbOCl.  Insol.  in  H20.     De- 
comp.  by  boiling  with  H20;  sol.  in  HCl+Aq. 

Tnsnl    in  alnnhnl  or  pfhpr'  «nl    in  f~!£L    nTTPl. 

(Schulze,  J.  pr.  (2)  27.  320.) 

Antimony  bisulphide  with  M2S. 
See  Sulphantimonites,  M. 

Antimony  pentasulphide,  Sb2S6. 

Insol.  in  H20,  or  H2O  containing  H2S.  Sol. 
in  cone.  HCl+Aq.  Completely  sol.  in 
NH4OH+Aq;  traces  dissolve  in  (NH4)2CO3  + 
Aq.  Easily  sol.  in  KOH,  or  NaOH+Aq,  or 
in  alkali  sulphides +Aq.  Sol.  in  50  pts.  cold 
dil.  NH4OH+Aq.  (Geiger.) 

Insol.  in  (NH4)2CO3+Aq. 

Insol.  in  cold,  but  sol.  in  hot  alkali  carbon- 
ates -fAq.  (Berzelius.) 

Insol.  in  Na3SbS4+Aq. 

When  boiled  with  alcohol,  ether,  CS2,  oil 
of  turpentine,  etc.,  portion  of  the  S  is  dis- 
solved out.  (Berzelius.) 

CS2  dissolves  about  5%  of  the  sulphur. 
(Rammelsberg.) 

Antimony  pewtasulphide  with  M2S. 
See  Sulphantimonates,  M. 

Antunony  sulphochloride,  SbSCl3. 

Decomp.  by  moist  air  or  H2O.  (Cloez.  A. 
ch.  (3)  30.  374.) 

SbS2Cl.  Easily  attacked  by  acids;  insol.  in 
CS2.  (Ouvrard,  C.  R.  116.  1516.) 

Sb2S5Cl.    (Ouvrard.) 

2SbSCl,  3Sb2S3.  Decomp.  by  dil.  HC1+ 
Aq.  (Schneider.) 

SbSCl,  7SbCl3.  Deliquescent;  decomp.  by 
H2O.  (Schneider,  Pogg.  108.  407.) 

Antimony  sulphofluoride,  SbF6S. 

See  Antimony  fluo sulphide. 
Antimony  sulphoiodide,  SbSI. 

Not  attacked  by  H2O,  and  decomp.  only 
by  cone,  acids.  Insol.  in  CS2.  (Schneider, 
Pogg.  110.  147.) 

Sb2S3Ie.    (Henry  and  Garot.) 

Sb2S2I3.  Sol.  in  dry  CS2.  Very  easily  de- 
comp. (Ouvrard,  C.  R.  117.  108.) 


or  C6H6.    (Sabanajew,  Zeit.  Ch.  1871.  204.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  826.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Sb4OsCl2.  Algaroth  powder.  Decomp.  by 
H2O.  Sol.  in  HCl+Aq  (Cooke,  Proc.  Am. 
Acad.  13.  1);  tartaric  acid+Aq.  (Schaffer. 
A.  152.  135.) 

Sb8OnCl2.    (Cooke.) 

Sb8OCl22. 

Sb41O50Cl23. 

From  SbCl5.  SbOCl3.  Deliquescent.  De- 
composed by  H2O.  Sol.  in  H2O.  (Daubrawa, 
A.  184.  118.) 

Does  not  exist.  (Anschutz  and  Evans.  A. 
239.  285.) 

Sb3OCli3.  Deliquescent.  Insol.  in  CS2; 
easily  sol.  in  tartaric  acid+Aq.  (Williams, 
C.  N.  24.  224.) 

Sb3O4Cl7.    (Williams.) 

SbO2Cl.    Decomp.  by  hot  H2O  into  HSbO3. 

Antimonyl  fluoride. 

From  SbF3.  Sb4O3F6.  Not  deliquescent. 
(Fliickiger,  Pogg.  87.  249.) 

Antimonyl  caesium  fluoride,  SbF4OH,  CsF. 
(Wells,  Am.  J.  Sci.  1901,  (4)  11.  456.) 

Antimonyl  sodium  fluoride,  SbOF3,  NaF+ 
H2O. 

Deliquescent.  Easily  sol.  in  HoO.  (Marig- 
nac,  A.  145.  239.) 

Antimonyl  iodide,  Sb4O6I2. 

Difficultly  sol.  in  solution  of  tartaric  acid 
or  tartrates.  Decomp.  by  HC1,  HNO3,  or 
H2SO4+Aq.  Easily  sol.  in  alkalies,  or 
(NH4)2S+Aq. 

SbOI.  Insol.  in  CS2.  (Cooke,  Proc.  Am. 
Acad.  (2)  6.  72.) 

Antimonyl  sulphide. 
See  Antimony  oxysulphide. 


ARSENIC  CHLORIDE 


53 


Argon,  A. 

100  cc.  H2O  dissolve  4.05  cc.  argon  at  13.9°. 
Critical  t  — 121 .6°  under  50.6  atmos.  Bpt.  - 
186.9°.  Sp.  gr.  19.9.  (Rayleigh,  C.  N.  1895, 
71.  51-62;  299-302;  C.  C.  1895.  467.) 

Coefficient  of  absorption  in  H2O  at  12°  = 
0.0394;  at  13.9°  =  0.0405.  (Ramsay,  Phil. 
Trans.  1895,  186.  A.  225.) 

Absorption  by  H20  at  t°. 


t° 

Coefficient  of  absorption 

0° 
10 
20 
30 
40 
50 

0.0561 
0.0438 
0.0379 
0.0348 
0.0338 
0.0343 

(Antropoff,  Roy.  Soc.  Proc.  1910,  83.  A.  480.) 

Absorption  of  argon  by  H20  at  t°  and  760 
mm.  pressure. 


t° 

Coefficient  of  absorption 

0° 

0.05780 

1 

0.05612 

5 

0.05080 

10 

0.04525 

15 

0.04099 

20 

0.03790 

25 

0.03470 

30 

0.03256 

35 

0.03053 

40 

0.02865 

45 

0.02731 

50 

0.02567 

(Estreicher,  Z.  phys.  Ch.  1899,  31.  184.) 

1 1.  H20  at  38°  absorbs  25.7  cc.  A. 

1  1.  blood  absorbs  25.3  cc.  A.  (Regnard 
and  Schloesing,  C.  R.  1897,  124.  303.) 

Not  absorbed  by  members  of  the  fatty 
series  of  organic  compounds;  with  members 
of  the  aromatic  series  absorption  was  ob- 
served varying  from  8%  of  the  volume  em- 
ployed for  benzene  to  1  %  for  aniline.  (Berth- 
elot,  C.  R.  1899,  129.  71.) 

Arsenamide,  As(NH2)3. 

Insol.  in  liquid  NH3.  Decomp.  by  H2O. 
(Hugot,  C.  R.  1904,  139.  55.) 

Arsenic,  As. 

Unaltered  by  pure  H2O.  Insol.  in  HC1  + 
Aq  if  air  is  excluded,  but  si.  sol.  in  presence  of 
air.  Not  attacked  by  dil.  H2SO4+Aq.  Oxi- 
dized by  cone.  H2SO4,  HNO3,  or  aqua  regia. 
Not  attacked  at  20°  by  HNO3,  cone,  or  dll., 
or  containing  NO2;  nor  by  HN03+HC1,  as 
long  as  they  do  not  act  on  each  other;  but  if 
treated  with  the  above  mixture  in  extremely 
dilute  state,  and  a  few  drops  of  KNO2+Aq 


are  added,  the  As  is  attacked  at  once.    (Mil- 
Ion,  A.  ch.  (3)  6.  101.) 

Sol.  in  sea  water;  0.009  mg.  per  liter  off 
Brittany;  0.01  to  0.09  mg.  per  liter  near 
Azores.  (Gautier,  C.  R.  1903,  137.  232.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Insol.  in  liquid  .NH3.  (Hugot,  A.  ch.  1900, 
(7)21.31.) 

Insol.  in  NaOH,  KOH,  or  NH4OH+Aq. 

Sol.  in  S2Br2.  (Hannay,  Chem.  Soc.  (2)  11. 
823.) 

Insol.  in  alcohol  and  ether. 

Sol.  in  certain  fatty  oils. 

Insol.  in  methylene  iodide.  (Retgers,  Z. 
anorg.  3.  343.) 

Yi  ccm.  oleic  acid  dissolves  0.0032  g.  As  in 
6  days.  (Gates,  J.  phys.  Ch.  1911,  15.  143.) 

Yellow  modification.  Very  unstable.  (Mc- 
Leod,  C.  N.  1894,  70.  139.) 

Fairly   stable   in   liquid   air.      (Thomson, 
Chem.  Soc.  1906,  90.  (2)  745.) 
100  ccm.  CS2  dissolve  at: 

46°    20°     12°     0°      —15°          —60° 

11        8        6      4      2.0-2.5     l.Og.  As. 

Less  sol.  in  benzene  and  ethyl  acetate. 
(Erdmann,  Z.  anorg.  1902,  32.  448.) 

Arsenic  acid.    See  page  59. 

Arsenic  bromide,  AsBr3. 

Decomp.  by  H2O.  Completely  sol.  in 
about  3  pts.  boiling  H2O,  and  much  less,  in 
presence  of  HBr.  (Wallace,  Phil.  Mag.  (4) 
17.  261.) 

Sol.  inCS2. 

Sol.  in  AlBr3.  (Isbekow,  Z.  anorg.  1913, 
84.  26.) 

Easily  sol.  in  PC13  and  PBr3.  (Walden, 
Z.  anorg.  1900,  25.  211.) 

Sol.  in  S2C12.  (Walden,  Z.  anorg.  1900, 
25.  217.) 

Arsenic  caesium  bromide,  2AsBr3,  3CsBr. 

Decomp.  by  H2O;  can  be  recryst.  from 
cone.  HBr+Aq.  (Wheeler,  Z.  anorg.  4.  451.) 

Arsenic  rubidium  bromide,  2AsBr3,  3RbCl. 
As  the  corresponding  Cs  comp. 

Arsenic  bromide  ammonia,  AsBr3,  3NH3. 

Decomp.  by  H2O.     (Besson,  C.  R.  110. 
1258.) 
Arsenic  bromide  copper,  2AsBr3,7Cu. 

Stable  toward  hot  H2O.  Decomp.  by  KOH. 
(Hilpert  andHernnan,  B.  1913,  46.  2224.) 

Arsenic  bromide  silver,  AsBr3,  3Ag. 

Scarcely  decomp.  by  cold  H2O.  (Hilpert 
and  Herrmann.) 

Arsenic  chloride,  AsCl3. 

Miscible  with  little  H2O,  and  with  alcohol, 
ether,  and  volatile  oils.  Decomp.  by  much 
H2O,  or  by  boiling.  (Gmelin.) 


54 


ARSENIC  CHLORIDE 


Miscible  with  oil  of  turpentine,  and  wit! 
olive  oil.  Somewhat  sol.  in  HCl+Aq. 

Easily  sol.  in  PC13  and  PBr3.  (Walden 
Z.  anorg.  1900,  26.  211.) 

Sol.  in  liquid  CN.  (Centnerszwer,  J.  russ 
phys.  Ges.  1901,  33.  545.) 

Sol.  in  SoCl2.  (Walden,  Z.  anorg.  1900,  25 
217.) 

Arsenic  penta  chloride,  AsCl5. 

Fumes  in  the  air  with  evolution  of  hydro 
gen  chloride.  Readily  sol.  in  CS2,  and  ab 
solute  ether  cooled  to  — 30°.  (Baskerville 
J.  Am.  Qhem.  Soc.  1902,  24.  1070.) 

Arsenic  caesium  chloride,  2AsCl3,  3CsCl. 

Decomp.  by  H2O.  100  pts.  HCl+Aq  (1.2 
sp.  gr.)  dissolve  0.429  pt.  salt.  (Wheeler 
Z.  anorg.  4.  451.) 

Arsenic  indium  phosphorus  chloride. 

See  Iridium  phosphorus  chloride  arsenic 
chloride. 

Arsenic  rubidium  chloride,  2AsCl3,  3RbCl. 

Decomp.  by  H2O.  100  pts.  HCl+Aq  (sp 
gr.  1.2)  dissolve  2.935  pts.  salt.  (Wheeler,  Z 
anorg.  4.  451.) 

Arsenic  sulphur  chloride,  2AsCl3,  3SC12. 

Decomp.  by  H2O.    (Rose.) 

Above  compound  is  a  mixture.  (Nilson 
C.  N.  81.  81.) 

Arsenic  chloride  ammonia,  2AsCl3,  7NH3. 

Decomp.  by  cold  H2O,  with  evolution  of 
NH3.  From  the  solution  crystallizes  As4CL 
N2H1008. 

Sol.  in  alcohol  without  decomp.  (Rose, 
Pogg.  52.  62.) 

Composition  is  AsCl3,  4NH3.  (Besson, 
C.  R.  110.  1258.) 

Arsenic  chloride  copper,  2AsCl3,7Cu. 

Somewhat  decomp.  by  H2O.  Decomp.  by 
KOH,  or  hot  HC1.  (Hilpert  and  Herrman, 

B.  1913,  46.  2224.) 

Arsenic  chloride  silver,  2AsCl3,  7Ag. 

H2O,  NH4OH  and  KOH  split  off  Ag.  (Hil- 
pert and  Herrmann.) 

Arsenic  influoride,  AsF3. 

Sol.  in  H2O  with  evolution  of  heat  and  de- 
composition. (Berzelius.) 

Easily  sol.  in  benzene.  (Moissan,  C.  R. 
99.  874.) 

Miscible  with  alcohol  and  ether.    (M'lvor, 

C.  N.  30.  169.) 

Arsenic  pewtafluoride,  AsF6. 

Sol.  in  H2O,  alkalies +Aq  and  liquid  AsF3 
with  evolution  of  heat.  Absorbed  by  ether, 
alcohol  and  benzene  with  evolution  of  heat 
(Ruff,  B.  1906,  39.  67.) 


Arsenic    potassium    fluoride,    AsF5,    KF  + 


AsF5,  2KF+H2O. 

AsF5,  AsOF3,  4KF+3H2O.  (Marignac,  A. 
145.  237.) 

Arsenic  fluoride  ammonia,  2AsF3,  5NH3. 

Easily  decomp,  by  H2O.  (Besson,  C.  R. 
110.  1258.) 

Arsenic  pewtofluoride  nitrosyl  fluoride,  AsF5, 
NOF. 

Decomp.  by  H2O,  fuming  HC1,  NaOH+Aq, 
dry  ether  and  dry  alcohol  with  evolution  of 
NO.  Sol.  in  cone.  HNO3,  hot  cone.  HoSO4, 
boiling  NOC1  and  AsF3.  Insol.  in  CC14  and 
CS2.  (Ruff,  Z.  anorg.  1908,  58.  327.) 


Arsenic    ^fluoride     sulphur 

2AsF3,  SC14. 
Very  hydroscopic.  Decomp.  by  H2O  and 
NaOH.  Decomp.  by  thionyl  chloride,  CC14, 
CS2,  abs.  alcohol  and  ether.  Decomp.  by 
ligroin,  benzene  and  toluene.  (Ruff,  B.  1904, 
37.  4520.) 

Arsenic  hydride,  AsH3. 

SI.  sol.  in  H2O  and  alkali  hydrates+Aq, 
with  subsequent  decomposition.  H2O  ab- 
sorbs Vs  vol.  AsH3.  Decomp.  by  cone,  acids. 
Absorbed  rapidly  by  oil  of  turpentine,  slightly 
by  fixed  oils,  and  not  at  all  by  alcohol,  ether, 
orKOH+Aq.  (Gmelin.) 

Insol.  in  KOH  +  Alcohol.    (Meissner.) 

Not  more  sol.  in  alkaline  solutions  than  in 
pure  H2O.  (Berzelius.) 

AsH.  Solid.  Insol.  in  H2O,  alcohol,  ether, 
and  CS2.  (Wiederhold,  Pogg.  118.  615.) 

Insol.  in  H2O;  sol.  in  methylene  iodide, 
cylene,  or  in  cone.  KOH+Aq.  (Retgers,  Z. 
anorg.  4.  403.) 

Arsenic  hydride  boron  bromide,  AsH3,  BBr3. 
Easily  decomp.     Decomp.  by.  H2O.     Ap- 
preciably sol.  in  AsH3  or  BBr3.    Insol.  in  CS2. 
Stock,  B.  1901,  34.  949.) 

Arsenic  (Modide,  As2I4. 

Decomp.  by  H2O  or  alkalies;  easily  sol.  in 

alcohol,  ether,  chloroform,  or  carbon  disul- 

hide.    (Bamberger  and  Phillip,  B.  14.  2643.) 

Not  attacked  by  cold  cone.  H2SO4  or  by 

sold  fuming  HNO3.     The  latter  oxidizes  on 

vanning.     Decomp.   by  pyridine.     Sol.   in 

soiling  acetic  anhydride.    (Hewitt  and  Win- 

mill,  Chem.  Soc.  1907,  91.  962.) 

Vrsenic  friiodide,  AsI3. 
Sol  in  3.32  pts.  boiling  H2O,  and  solution 
boiled  down  deposits  pure  AsI3,  but  if  left 

o  cool  slowly,  deposits  crystals  of  As2O3  and 

LfiUl. 

SI.  sol.  in  HCl+Aq. 

Sol.  in  POC1S,  PC13  and  PBr3.     (Walden, 
r.  anorg.  1900,  25.  212.) 


ARSENIC  OXIDE 


55 


Sol.  in  PC13.  (Beckmann,  Z.  anorg.  1906 
61.  110.) 

Sol.  in  SOC12,  S2C12  and  S02C12.  (Walden 
Z.  anorg.  1900,  25.  216.) 

Sol.  in  SnCl4.    (Walden,  I.e.} 

Easily  sol.  in  AsBr3.  (Walden,  Z.  anorg 
1902,  29.  374.) 

Sol.  in  AsCl3.  (Walden,  Z.  anorg.  1900 
26.  214.) 

Sol.  in  alcohol  without  decomp. 

Sol.  in  ether,  benzene,  chloroform,  and  CS2 

100  pts.  methylene  iodide  dissolve  17.4  pts 
AsI3  at  12°.  (Retgers,  Z.  anorg.  3.  343.) 

Arsenic  pentaiodide,  AsI5. 

More  or  less  sol.  in  H2O,  alcohol,  CHC13 
ether  and  CS2.  (Sloan,  C.  N.  1882,  46.  194.. 

Arsenic  caesium  iodide,  2AsI3,  3CsI. 

Decomp.  by  H2O;  sol.  in  cone.  HI+Aq 
(Wheeler,  Z.  anorg.  4.  451.) 

Arsenic  rubidium  iodide,  2AsI3,  3RbI. 

As  the  corresponding  Cs  comp. 
Arsenic  sulphur  iodide. 

See  Arsenic  sulphoiodide. 
Arsenic  Zraodide  ammonia,  2AsI3,  9NH3. 

Insol.  in  benzene.  (Bamberger  and  Phillip 
B.  14.  2643.) 

Asl,,  4NH3.    (Besson,  C.  R.  110.  1258.) 

Arsenic  nitride,  AsN. 

Easily  decomp.  into  As  and  N.  (Hugot,  C, 
R.  1904,  139.  56.) 

Decomp.  by  heat.  (Franz  Fischer,  B. 
1910,  43.  1471.) 

Arsenic  sw&oxide,  As2O  (?). 

Insol.  in  H2O;  decomp.  by  dil.  acids  or 
NH4OH+Aq. 

Does  not  exist.    (Geuther,  A.  240.  208.) 

Arsenic  fnoxide,  As2O3. 

"White  arsenic"  exists  in  two  modifica- 
tions: aAs2O3, — crystalline,  octahedral, 
opaque,  porcelaneous,  etc.;  /3As2O3, — amor- 
phous, vitreous,  "arsenic  glass." 

The  data  concerning  the  solubility  of  As2O3 
are  very  contradictory,  the  reasons  being  that 
(1)  the  solubility  of  the  two  modifications  is 
different;  (2)  that  the  length  of  time  necessary 
to  effect  solution  differs  in  the  two  modifica- 
tions; and  (3)  that  there  is  a  tendency  of  the 
amorphous  As2O3  to  go  over  into  the  crystal- 
line state  during  the  process  of  solution. 
aAs2O3  is  also  not  easily  moistened,  especially 
when  in  a  pulverulent  condition,  which  is  not 
the  case  with  the  p  modification.  (Winkler, 
J.  pr.  (2)  31.  247.) 

The  older  data  are  very  unreliable,  but  pos- 
sess a  certain  historical  interest. 

1  pt.  As2O3  is  sol.  in  10.55  pts.  (Wenzel);  11.34 
pts.  (Fischer);  11.86  pts.  in  %  hour  (Klaproth);  12.2 
pts.  (Bucholz);  15.0  pts.  (Brandt;  Bergman);  16.0  pts. 
(Vogel) ;  24  pts.  (Lametherie) ;  40  pts.  (Porner) ;  64  pts. 


(Baume) ;  80  pts.  (Navier) ;  200  pts.  (Aschof  and  Nasse, 
1812) ;  640  pts.  (Hagen,  1796)  boiling  H2O. 

1  pt.  As2Os  is  sol.  in  7.72  pts.  H2O  if  a,  or  9.33  pts.  if 
j8  (Guibort) ;  in  24  pts.  HjO  if  a,  or  21  pts.  if  0  (Taylor). 
Sol.  in  53.3  pts.  H2O  at  18.75°.    (Abl.) 
Sol.  in  30  pts.  H2O.    (Nussembrock.) 
After  the  solution  in  H2O  at  100°  has  been  left  stand- 
ing at  ordinary  temperatures — 

1  pt.  As2O3  remains  dissolved  in  16  pts.  H2O  at  16°, 
and  20  pts.  H2O  at  7°  (Bucholz) ;  in  33  pts.  H2O  at  7° 
(Klaproth) ;  in  38.45  pts.  H2O  after  3  days,  55  pts.  H2O 
after  8  days,  64.50  pts.  H2O  after  2.3  weeks  at  10° 
(Fischer) ;  in  33.52  pts.  if  aAs2O3  was  used,  55.06  pts.  if 
jSAszOs  was  used  (Guibort) ;  in  38  pts.  if  aAs2Os  after  6 
months,  53.71  pts.  if  #As2O3  after  48  hours  (Taylor). 

When  an  excess  of  pulverized  As2Os  is  left  to  digest 
for  several  days  with  cold  H2Q — 

1  pt.  dissolves  in  50  pts.  (Bucholz);  in  66  pts. 
(Fischer) ;  in  80  pts.  at  15°  (Bergman) ;  in  80  pts.  if  a, 
and  103  pts.  if  /3  (Guibort) ;  96  pts.  at  10°  (Spelman) ; 
96  pts.  at  35.5°  (Hahnemann);  320  pts.  H2O  at  20° 
(Aschof  and  Nasse,  1812.) 

H2O  at  15.6°  or  below  dissolves  less  than  Y±%  AszOj. 
(Dalton.) 

To  dissolve  1  pt.  As2C>3  in  12  pts.  H20,  it  is  necessary 
to  boil  an  excess  of  As2O3  with  H2O;  if  1  pt.  As2Os  is 
boiled  with  12  pts.  H2O,  considerable  remains  undis- 
solved;  and  even  with  1  pt.  As2O3  to  50-60  pts.  H2O 
long  continued  boiling  is  necessary  to  effect  solution. 
If  a  clear  solution  saturated  by  long  boiling  with  an 
excess  of  As2O3  is  poured  off  and  evaporated  con- 
tinuously to  %  its  original  bulk,  no  As2O3  separates 
out,  and  the  solution  contains  1  pt.  As2O3  to  6  pts.  H2O. 
(Fischer.) 

100  pts.  aqueous  solution  of  /3As2Os  sat.  at  15°  con- 
tain 0.96  pt.  AssOs,  and  9.68  pts.  when  sat.  at  100°. 
(Guibort.) 

If  1  pt.  pulverized  As2O3  be  digested  10  days  at  19-25° 
in  5-10  pts.  H2O,  the  solution  contains  1  pt.  As2O3  to  50 
pts.  H2O.  A  solution  of  same  strength  is  obtained  in 
25  days  by  digesting  1  pt.  As2O3  in  40  pts.  H2O.  If  1 
pt.  As2O3  be  immersed  in  80  pts.  H2O,  the  resulting 
solution  contains  1  pt.  As2Os  to  90  pts.  H2O;  if  in 
160  pts.  H2O,  1  pt.  As2O3  to  180  pts.  H2O;  if  in  240 
pts.  H2O,  1  pt.  As2O3  to  280  pts.  H2O;  if  in  1000  pts. 
H2O,  1  pt.  As2Os  to  1200  pts.  H2O;  and  even  when  1 
pt.  As2Os  is  digested  at  ordinary  temperatures  for 
several  days  with  16,000-100,000  pts.  H2O,  a  portion 
remains  undissolved.  Pulverized  aAs2O  iwas  set  aside 
with  H2O  in  closed  bottles  for  18  years;  when  1  pt. 
As2Os  was  present  in  1000  pts.  H2O,  a  perfect  solution 
was  obtained;  when  1  pt.  As2O3  in  100  pts.  H2O,  0.017% 
As2O3  was  undissolved;  when  1  pt.  As2Os  in  35  pts. 
H2O,  0.35%  As2Os  was  undissolved,  so  that  the  solution 
contained  1  pt.  As2O3  to  54  pts.  H2O.  (Gmelin.) 

Porcelaneous  modification  (aAs2O3)  is  much  more  sol. 
in  H2O  than  the  vitreous  (/3As2O3).  100  pts.  H2O  at 
ordinary  temperature  dissolve  0.96  pt.  BAs2O3  and  1.25 
pts.  oAs2Os;  100  pts.  boiling  H2O  dissolve  9.68  pts. 
?As2Os  and  11.47  pts.  aAs2O3;  and  when  the  tempera- 
;ure  of  this  solution  has  fallen  to  15°,  the  solution  from 
/3As2Os  retains  1.78  pts.,  and  that  from  aAs2Oj  retains 
2.9  pts.  (Berzelius  [citing  Guibort].) 

/8As2O3  dissolves  more  quickly  and  abun- 
dantly than  aAs2O3.  The  same  amount  H2O 
which  will  take  up  36-38  pts.  £As2O3  at  12- 
3°  will  dissolve  only  12-14  pts.  aAs2O3,  or 
00  pts.  H2O  dissolve  4  pts.  /3As2O3  and 
.2-1.3  pts.  aAs2O3.  By  long  boiling  with 
52O,  aAs2O3  is  converted  into  /3As2O3,  and 
hus  acquires  the  solubility  of  the  latter,  so 
hat  100  pts.  boiling  H2O  can  take  up  11  pts. 
Ls2O3.  But  at  low  temperature  /3As2O3  is 
onverted  into  aAs203  when  in  contact  with 
H2O,  so  that  the  solution  becomes  weaker 
fter  a  while,  and  retains  only  the  proportion 
f  As2O3  corresponding  to  the  solubility  of 
As203.  Comminution,  which  hastens  the 
ate  of  solubility  of  aAs2O3  without  increasing 
he  amount  dissolved,  diminishes  the  solubil- 
;y  of  0As2O3,  as  this  is  converted  into  aAs2O3 


56 


ARSENIC  OXIDE 


by  the  friction  or  contact  with  H20.  As2O3, 
which  has  been  rendered  opaque  by  NH4OH, 
and  that  which  has  been  crystallized  from  an 
aqueous  solution,  are  equally  sol.  in  H2O. 
(Bussy,  C.  R.  24.  774;  A.  64.  286.) 

100  pts.  H2O  dissolve  1.707  pts.  /3As2O3  in 
2H  years;  100  pts.  boiling  H2O  dissolve  11.46 

Ets.  0As2O3  in  3  hours,  and  11.86  pts.  in  12 
ours;  10.14  pts.  aAs203  in  3  hours,  and  10.18 
pts.  in  12  hours.     (Rose,  Ann.  Phys.  (1)  36. 
494.) 

A  cold  sat.  solution  which  stood  over  excess 
of  As2O3  for  10  months  at  10-20°  contains 
1.2%  As203;  hot  sat.  solution  a  few  days  after 
saturation  contains  2.25-2.50%  As203.  If 
trace  of  HC1  is  present,  the  solution  contains 
3.8%  As203.  Hot  sat.  solution  of  porcelain 
mod.  of  As2O3  contains  4  days  after  satura- 
tion 2.4%  As203  at  24°;  after  82  days  at  14°, 
1.5%;  after  4  months  at  12°,  1.3%  As203. 
(Bacaloglo,  J.  pr.  83.  111.) 

According  to  later  experiments,  1  pt.  aAs2O3 
dissolves  in  355  pts.  H2O  in  1  day  at  15°, 
while  1  pt.  j8As2O3  dissolves  in  108  pts.  H2O 
under  the  same  conditions.  1  pt.  aAs203  dis- 
solves in  46  pts.  H20,  if  solution  is  prepared 
at  100°,  and  allowed  to  stand  24  hours  at  15°, 
while  1  pt.  /SAs2O3  dissolves  in  30  pts.  H2O 
under  the  same  conditions.  (Biichner,  N. 
Rep.  Pharm.  22.  265.) 

100  pts.  H2O  dissolve  pts.  aAs203  and  /3As2O3 
at  ordinary  temperature: 


Ratios  of 

t° 

Pts. 

+  ° 

Pts. 

amts.  dis- 

jSAsaOs 

/3As2O3 

solved  at 

80°  :  18.5° 

80° 

1.0195 

18.5° 

0.5422 

1.88      1 

1.3664 

0.7203 

1.89     1 

1  .  1933 

.... 

0.6522 

1.84     1 

In  the  solution  of  /3As2O3,  octahedral  crys- 
tals were  deposited  on  the  sides  of  the  vessel 
after  12  hours,  which  continued  to  increase. 
There  was  no  such  deposit  in  the  case  of 
aAs2O3. 

From  the  maxima  in  the  above  table,  100 
pts.  H2O  can  dissolve  3.7  pts.  £As2O3  and  1.7 
pts.  aAs2O3  at  ordinary  temperature. 

100  pts.  boiling  H2O  dissolve  11.46  pts. 
/3As2O3  and  10.140  pts.  aAs2O3  in  3  hours; 
11.86  pts.  /3As2O8  and  10.176  pts.  aAs2O  in 
12  hours.  (Cl.  Winkler,  J.  pr.  (2)  31.  247.) 

100  pts.  H2O  dissolve  1.75  pts.  of  a  third 
modification  (hexagonal  crystalline)  at  or- 
dinary temperature,  and  2.75  pts.  at  100°. 
(Claudet,  Chem.  Soc.  (2)  6.  179.) 

|9As203  dissolves  more  rapidly  in  HCl-f  Aq 
than  aAs2O3.  (Schultz-Sellac,  B.  4.  109.) 


While  100  ccm.  H2O  dissolve  0.8507  g. 
/3As203  at  18.5°,  100  ccm.  H2O  containing 
1.3195  g.  HC1  dissolve  1.1513  g.  j3As2O3; 
containing  6.09  g.  HC1,  1.2724  g.  /3As2O3. 
(Chodounsky,  Listy  Chemicke",  13.  114.) 

100  ccm.  H2O  dissolve  1.495  g.  As2O3  at 
15°.  (W?od,  Chem.  Soc.  1908,  93.  412.) 

Solubility  of  crystalline  As2O3  in  H2O. 

1  1.  of  the  sat.  solution  contains  at: 

2°          15°       .25°       39.8°  bpt. 

12.006  16.566  20.384  29.302  60+g.  As2O3 
(Bruner,  Z.  anorg.  1903,  37.  456.) 

Much  more  easily  sol.  in  many  acids  than 
in  H2O.  Easily  sol.  in  fuming  H2SO4. 
(Schultz-Sellac.) 

100  pts.  dilute  H2S04+Aq  of  various 
strengths  dissolve  at  t°. 


(Chodounsky,  I.e.] 

Decomp.  by  HNO3  or  aqua  regia  into  As2O6. 
Sol.  in  H3P04+Aq.    (Bergman.) 
More  sol.  in  HCl+Aq  than  in  H2SO4,  or 
HNO3+Aq,  and  still  less  in  HC2H3O2+Aq. 
Solubility  in  HCl+Aq. 


Time 

aAsiOs 

/3As203 

Cone,  of  HCl+Aq 

Grams  of  As2Os  per  100  cc. 
of  solution 

1  hour 

0.023 

1.589 

3  hours 

0.088 

2.356 

0  46N 

1  52 

6  hours 

0.353 

3.666 

0  98N 

1  41 

12  hours 

0.364 

3.361 

2  03N 

1  17 

24  hours 

0.956 

3.306 

3  13N 

1  11 

2  days 

1.627 

2.629 

3  81N 

1  13 

4  days 

1.814 

2.429 

5  32N 

2  20 

1  week 

1.673 

1.763 

6  SON" 

5  11 

3  weeks 

1.776 

1.713 

7.85N 

12.28 

2M  years 

1.712 

1.707 

9.17N 

18.16 

As  the  concentration  of  the  acid  increases, 
the  solubility  of  the  oxide  decreases,  a  mini- 
mum being  reached  when  the  concentration 
of  the  solvent  is  about  3.2N.  Beyond  this 
point,  an  increase  in  the  concentration  of  the 
solvent  leads  to  a  corresponding  increase  in 
the  solubility.  (Wood,  Chem.  Soc.  1908,  93. 
413.) 

Insol.  in  liquid  CO2.  (B.uchner,  Z.  phys. 
Ch.  1906,  64.  674.) 

Easily  sol.  in  cold  H2C204+Aq.  (Berg- 
man.) 

When  pulverized,  it  dissolves  in  hot  H2C2O4 
+Aq,  but  separates  out  on  cooling. 

Easily  sol.  in  hot  benzoic  acid+Aq. 

Sol.  in  tartaric  acid+Aq. 

Easily  sol.  in  alkali  hydrates,  or  carbonates 
+Aq. 


ARSENIC  OXIDE 


57 


Easily  sol.  in  NH4  arsenite+Aq  at  70-80°, 
crystallizing  out  on  cooling.    (Berzelius.) 
Sol.  in  hot  K2C2O4+Aq. 
Sol.  in  AsCl3.    (Penney  and  Wallace.) 
More  sol.  in  Na2B4O7-|-Aq  than  in  H2O. 
Very  si.  sol.  in  absolute  alcohol.    (Vogel.) 

Sol.  in  80  pts.  highly  rectified  spirit.     (Wenzel.) 
When  1  pt.  powdered  As2Os  is  digested  30  days 
10-40  pts.  alcohol,  a  solution  is  formed  containing  1  pt. 
As2Os  to  60  pts.  alcohol;  when  1  pt.  As2Oa  is  digestec 
with  60-150  pts.  alcohol,  a  solution  is  formed  containing 
1  pt.  AszOs  to  124-140  pts.  alcohol.     (Fischer.) 
Sol.  in  70-80  pts.  alcohol.     (Thompson.) 

Alcohol  dissolves  0.446  pt.  /3As2O3.    (Rose, 


Arsenic  trioxide   pentoxide,   3As2O3,   2As2O5 

+3H2O. 

Decomp.  by  H2O.    (Joly,  C.  R.  100.  1221.) 
2As2O3,  As->O5+H,O.     Decomp.  bv  H2O. 

(Joly.) 
As2O3,  As205+H2O.    (Joly.) 

Arsenic  tefroxide,  As204. 

SI.  sol.  in  H2O  from  which  it  is  partially 
pptd.  by  alcohol.  More  easily  sol.  in  alkali 
carbonates  or  HCl+Aq.  Most  easily  sol.  in 
NaOH  or  KOH+Aq.  (Herbst,  Dissert. 
1894.) 


A.  I'nys. 

(i)  oz.  loo.; 

Arsenic  pewtoxide,  As2O5. 

100  pts 

.  alcohol  dissolve  pts.  As2O3: 

Deliquescent  in  moist  air;  slowly  sol.  in 

TT    f~\      fnrt-mi-nrr    TT      A  Of~\         TTrVkirtVi    n^k^ 

TP^^.1-.,.  ^^.1 

Vol.  %  of 
alcohol 

aAsaOs  at 
15° 

b.-pt.    of 
alcohol 

jSAsaOs  at 
15° 

-Cl2vJ',  lOIIillllg  Jl3rVSvy4,  wniCIl  See.       -Ljaoj^y   oui. 

in  alcohol;  much  more  sol.  in  alcohol  than 
As2O3.     Very  si.  sol.  in  the  fatty  oils,  100  pts. 
of  oil  dissolving  0.2  pt.  As2O5  in  the  cold,  and 

56 

1.680 

4.895 

0.504 

1  pt.  with  partial  decomp.  on  boiling.    (Ber- 

79 
84 
86 

88 

1.430 

0^715 

4.551 
3.'  197 

0.540 
0.565 

0'717 

zelius.) 
1000  pts.  boiling  poppy-oil  dissolve  27  pts. 
As2O5;  1000  pts.  boiling  castor-oil  dissolve  34 
pts.  As2O5.    (Heimpel  and  Grundner.) 

100 

0^025 

3.  '402 

1.060 

+4H2O.    Solubility  in  H2O  at  t°. 

(Girardin,  J.  Pharm.  (3)  46. 

269.) 

t° 

Pts.   HaAsCU 
inlOO  pts. 

t° 

Pts.  HjAsO4 
in  100  pts. 

100  pts 

absolute  alcohol  dissolve  0.446  pt. 

solution 

solution 

/3As2O3  in 

2M  years. 

(Winkler,  J.  pr.  (2)  31. 

—55° 

69.9 

CO 

80.0 

347.) 
Nearly 
100  pts 

insol.  in  ether. 
.  ether  dissolve  0.454 

pt.  |8As203. 

—50 
—45 
—40 

70.9 
71.9 
72.9 

0 

+5 
10 

81.0 
82.1 
83.3 

(Winkler.j 

Qfv 

73  Q 

15 

84  7 

Ether    extracts    1    mg.    As2O3    from    sat. 
As2O3+Aq  for  every  15  cc.  ether  used;  less 
is  extracted  when  the  solution  is  acidified 
with  HC1,  and  almost  none  if  acidified  with 

O<J 

—30 
—25 
—20 

1  K 

4  O  .  i7 

74.9 
75.9 
76.9 

77  Q 

20 
25 
30 

Q^ 

86^3 
88.0 
90.1 

OO    Q 

H2SO4  or 

H2C4Q6.    (Selmi,  B.  13. 

206.) 

XtJ 

.in 

V  •   »  V 

70  q 

OO 

•     —    .  O 

aAs2O3  is  sol.  in  50  pts.  boiling  nitrobenzol. 

Q  4          f~\        "        *              1       *         "U      '1*                   *J_         I*                   1       /  A 

l.\J 

1  O  .  t7 

pAs2O3  is  insol.  in  boiling  nitrobenzol.  (Auer- 
bach,  Z.  anorg.  1903,  37.  353.) 

(Menzies  and  Potter,  J.  Am.  Chem.  Soc.  1912, 

/3As2O, 

dissolves  in 

oil  of  turpentine,  but 

34.  1464.) 

aAs2O3  is  insol.  therein.     aAs2O3  is  very  si. 

Qnl     in   Vifvn  '/one*  AT  T"»o-fT*Al*viim    o'fViot*     VkiTf   THATA 

+5/3H2O.   Solubility  in  H2O  at  t°. 

HU1.    Ill    Ut>LlZ"Ht>   Ul    JJcul  OltyLlIIl   t5ullt?lj    LJUU   lllUltJ 

sol.  in  methyl  alcohol,  ethyl  alcohol,  ether, 

t° 

Pts.  HaAsO 

4  in  100  pts. 

or  chloroform.    (Selmi.) 

of  solution 

100  pts. 

USj  dissolve  0.001  pt 

/3As208  in 

1     1  AO 

OO 

2M  years. 

(Winkler.) 

+  10 

f\f\ 

88. 

o  f\ 

81.  sol.  in  the  fatty  oils. 

20 

on 

89. 

QQ 

• 

1000  pts.  castor-oil  dissolve  1.33  pts.  As2O3 

oO 

oy  . 
f\r\ 

at  ordinary  temperature,  and  9  pts.  at  boiling 

40 

K(\ 

90. 

Q1 

• 

0 

temperature.     1000  pts.  other  oils  dissolve 
0.6-0.8  pt.  As2O3  in  the  cold,  and  about  1.7 

O(J 

60 

7rt 

•  'I  .  _ 

91.9 

Q9   A 

pts.  on  boiling.    (Berzelius.) 
Insol.  in  chinoline  or  aniline.    (Hoffmann, 

/u 

80 
on 

y,<5.o 
93.2 

QO     Q 

A.  ch.  (3) 

9.  143.  169.1 

. 

yu 

y«j  .  o 

a  A     4 

Moderately  sol.  in 

chinolin.     (Beckmann 

100 

94.4 

f\K     f\ 

and  Gabel,  Z.  anorg.  1906,  51.  236.) 

110 
i  f)f\ 

95.0 

Qr    (\ 

Insol.  in 

acetone.    (Naumann,  B.  1904,  37. 

LZO 
i  QH 

yo.o 

Qfi    9 

4329);  (Eidmann,  C.  C.  1899,  II.  1014.) 
Sol.  in  amyl  alcohol  and  is  divided  between 

*j.     _„.  J     TT   /~\   *i,^     J.1-  _             ,-  -.4.  ~  «  4.     ><n4-ir\     rvf     1     •    ^\  AJ7 

lou 
140 

yo  .  z 
96.8 

it  ana  xi2U  in  tne  constant  ratio  01  i  .  o,rt/ 
at  25°.    (Auerbach,  Z.  anorg.  1903,  37.  376.) 

(Menzies  and  Potter,  J.  Am.  Chem.  Soc.  1912, 

Min.  Arsenolite. 

«i4.  14O4.; 

58 


ARSENIC  OXIDE 


As2O6+4H2O  and  3As2O5+5H20  are  the 
only  hydrates  that  can  be  isolated.  (Menzies 
and  .Potter.) 

See  also  Arsenic  Acid. 

Arsenic  <noxide,  with  alkali  haloid. 
See  Arsenite,  alkali  haloid. 

Arsenic  sulphur  fnoxide,  As2O3,  SO3. 

Deliquescent;    decomp.    by   H2O.     (Adie, 

Chem.  Soc.  55.  157.) 

As2O3,  2SO3.    As  above.    (Adie.) 
As2O3,  3S03.    (Weber,  B.  19.  3186.) 
As2O3,  4SO3.    As  above.    (Adie.) 
As2O3,  6SO3.    (Weber.) 
As2O3,  8SO3.    As  above.    (Adie.) 

Arsenic  oxychloride,  etc. 
See  Arsenyl  chloride,  etc. 

Arsenic  phosphide,  AsP. 

Decomp.  by  H2O.  Not  attacked  by  cold 
H2SO4  or  HC1,  and  only  si.  sol.  therein  on 
warming.  Easily  decomp.  by  HNO3,  KOH, 
NaOH,  BaO2H2+Aq.  Insol.  in  alcohol, 
ether,  chloroform;  si.  sol.  in  CS2. 

P2As302.  Product  of  action  of  H2O  on 
above  compound,  which  it  resembles.  (Jan- 
owsky,  B.  6.  216.) 

Arsenic  raowoselenide,  As2Se. 

Insol.  in  most  organic  and  inorganic  sol- 
vents. Sol.  very  slowly  in  cone.  HC1  and 
H2SC>4.  Sol.  in  boiling  alkali  hydroxides +Aq. 
(Szarvasy,B.  1897,  30.  1245.) 

Arsenic  tfnselenide,  As2S3. 

Partially  sol.  in  KOH+Aq  if  boiled  with  it 
for  a  long  time.  (Uelsmann,  A.  116.  123.) 

Arsenic  pentoselenide,  As2Se5. 

Insol.  in  most  solvents,  as  cone.  HC1.  Sol. 
in  alkali  hydrates  and  sulpho-hydrates+Aq. 
(Szarvasy,  B.  1895,  28.  2655-2656.) 

Insol.  in  H2O,  in  dil.  acids  and  in  cone.  HC1. 
SI.  sol.  in  warm  HNO3+Aq.  Oxidized  by 
cold  fuming  HNO3.  Sol.  in  alkalies  and  in 
hot  alkali  carbonates +Aq.  Insol.  in  alcohol, 
ether,  CS2,  etc.  (Clever,  Z.  anorg;  1895,  10. 
129.) 

Arsenic  selenosulphide. 

See  Arsenic  sulphoselenide. 
Arsenic  sulphide,  As3S. 

Ppt.  Insol.  in  NH4OH  or  in  colorless 
(NH4)2S+Aq.  Sol.  in  yellow  NH4SH+Aq. 
(Scott,  Chem.  Soc.  1900,  77.  652.) 

Arsenic  cftsulphide,  As2S2. 

Min.  Realgar.  Difficultly  sol.  in  alkali 
sulphides +Aq.  Partly  dissolved  by  KOH+ 
Aq  with  decomposition.  Sol.  at  150°  in  a 
sealed  tube  in  NaHCO3+Aq,  and  crystallizes 
out  on  cooling.  (SenarmOnt,  A.  ch.  (3)  32. 
158.) 


Arsenic  bisulphide,  As2S3. 

Insol.  in  H2O  when  prepared  in  the  dry  way, 
but  when  prepared  moist  is  very  liable  to  go 
into  the  colloidal  modification  mentioned 
below.  Insol.  in  H2O  containing  H2SO4 
HNO3,  HC1,  H2C2O4,  HC2H3O2,  H2C4H4O6, 
C02,  NH4C1,  KN03,  (NH4)2S04,  MgSO4. 
(Bontigny.) 

Insol.  in  H2O.  Traces  are  dissolved  by 
H2S+Aq.  SI.  decomp.  by  boiling  with  H2O, 
or  long  contact  with  cold  H2O.  (Fresenius.) 

1  1.  H2O  dissolves  2.1  x  10-6  mols.  pptd. 
As2S3  at  18°.  (Weigel,  Z.  phys.  Ch.  1907,  58. 
294.) 

Insol.  in  dil.  acids.  Insol.  in  cold,  and 
scarcely  attacked  by  hot  cone.  HCl+Aq. 

Easily  decomp.  by  HNO3  or  aqua  regia. 

Easily  sol.  in  cold  KOH,  NaOH,  or  NH4OH 
+Aq,  also  in  alkali  carbonates,  or  sulphates + 
Aq. 

Sol.  in  hot  KHSO3+Aq. 

Sol.  in  citric  acid,  and  alkali  citrates +Aq. 
(Spiller.) 

Slowly  sol.  in  cold  2%  Na2B4O7+Aq. 
Easily  sol.  on  heating.  (Materne,  C.  C.  1906, 
II.  557.) 

Insol.  in  CS2. 

Min.  Orpiment. 

As2S3  may  also  be  obtained  in  a  colloidal 
form,  sol.  in  H2O.  Sat.  solution  contains 
34.46%  As2S3;  it  is  decomp.  by  standing,  but 
may  be  boiled  without  undergoing  decom- 
position; most  acids  and  many  salts  ppt.  As2S3 
(Schulze,  J.  pr.  (2)  25.  431.) 

The  following  solutions  cause  pptn.  of 
As2S3  in  a  .solution  of  the  colloidal  modifica- 
tion, when  added  in  the  given  state  of  dilu- 
tion:— 

1  :  555 
1  :276 
1  :  255 
1  :  138 
1  :65 
1  :26 
1  :  0.18 
1  :76 
1  :  129 
:  188 
:2780 
:  2630 
:  3330 
:2860 
:3440 
:2380 
52600 


HCl+Aq 
HNO3+Aq     . 
H2S04+Aq     . 
H2S03+Aq     . 
H2C2O4+Aq  . 
H3P04+Aq    . 
HC2H3O2+Aq 
K2SO4+Aq    . 
Na2S04+Aq  . 
(NH4)2S04+Aq 
CaSO4+Aq    . 
MgSO4+Aq  . 
ZnS04+Aq    . 
MnSO4+Aq  . 
NiSO4+Aq     . 
FeS04+Aq     . 
Al2(S04)3+Aq 
Tl2S04+Aq    . 
KCl+Aq 
KBr+Aq 
KI+Aq . 
Lil+Aq 
NaCl+Aq      . 
NH4Cl+Aq   . 
BaCl2+Aq     . 
CaCl2+Aq     . 
MgCl2+Aq    . 


799 

137 

103 

55 

127 

212 

207 

2860 

4370 

10000 


ARSENIC  ACID 


59 


FeCls+Aq      . 
AlCl8+Aq      . 
CrCla+Aq      . 
KNOa+Aq     . 
NaNOs+Aq  . 
NH4NO3+Aq 
Ba(NO3)2+Aq 
KC103+Aq    . 
CaH2(C03)2+Aq   . 
K2G2H406+Aq       . 
K2CoO4+Aq  .      "..-•' 
NaC2H3O2+Aq      . 
Urea+Aq 

(NH4)2Fe(SO4)2+Aq 
K2Al2(SO4)4+Aq  . 
K2Fe2(SO4)4+Aq  . 
K2Cr2(S04)4+Aq  . 
K4Fe(CN)6+Aq  . 
K3Fe(CN)G+Aq  . 


1  :  50000 
1  :  83000 


:  20000 
:84 
:  117 
:  138 
:2080 
:88 
:  3120 
:85 


1  :78 
1  :25 
1  :  1160 
1  :  50000 
1  :  55500 
1  :  25000 
1  :67 
1  :81 


Cold  cone,  solutions  of  boric,  arsenious,  tar- 
taric,  benzoic,  and  salicylic  acids,  also  cane 
sugar,  or  chloral  hydrate  cause  no  pptn.  Ab- 
solute alcohol  and  glycerine  may  also  be 
mixed  with  the  solutions  without  causing 
pptn.  (Schulze,  J.  pr.  (2)  25.  442.) 

+6H2O;  decomp.  completely  into  As2S3 
under  a  pressure  of  6000  to  7000  atmos. 
(Spring,  Z.  anorg.  1895,  10.  186.) 

Arsenic  pewfa  sulphide,  As2S5. 

Insol.  in  H2O.  Sol.  in  NH4OH,  KOH, 
NaOH+Aq,  and  solutions  of  alkali  sulphides 
and  carbonates.  Sol.  in  BaOoH2,  and  Ca02H2 
+Aq. 

Sol.  in  citric  acid,  and  alkali  citrates +Aq. 
(Spiller.) 

Alcohol  dissolves  out  S  on  boiling.  (Ber- 
zelius.) 

Sol.  in  alkali  arsenates+Aq.  (Nilson,  J. 
pr.  (2)  14.  155.) 

+H2O.    (Nilson,  I.e.} 

Arsenic  bisulphide,  with  M2S. 
See  Sulpharsenites,  M. 

Arsenic  pentasulphide,  with  M2S. 
See  Sulpharsenates,  M. 

Arsenic    sulphobromide,    AsS2Br3=AsSBr+ 

SBr2. 

Decomp.  by  H2O.  (Hannay,  Chem.  Soc. 
33.  284.) 

Arsenic  sulphochloride,  As2S5Cl. 

Slowly  decomp.  by  boiling  H2O.  Sol.  in  hot 
AsCl3  without  decomp.  •  (Ouvrard,  C.  R.  116. 
1516.) 

AsS2Cl.  Decomp.  by  H2O.  Sol.  in 
NH4OH,  and  alkali  carbonates +Aq.  (Ouv- 
rard.) 

AsS2Cl.  Slowly  decomp.  by  boiling  H2O. 
Sol.  in  alkali  carbonates  and  in  NH4OH+Aq. 
(Ouvrard,  C.  R.  1893,  116.  1517.) 

Arsenic  sulphoiodide,  AsSI. 

Insol.  in  alcohol,  chloroform  or  carbon  di- 
sulphide.  (Schneider,  J.  pr.  (2)  23.  486.) 

Formula  is  probably  As2S3,  AsI3. 


Slowly  attacked  by  HCl+Aq;  somewhat 
more  easily  by  HNO3+Aq.  Easily  sol.  in 
KOH,  or  NH4OH  +  Aq.  (Schneider,  J.  pr.  (2) 
34.505.) 

2AsIs,  Sle.  Decomp.  on  air.  (Schneider, 
J.  pr.  (2)  36.  509.) 

As4S5I2.  Less  sol.  in  CS2  than  AsI3.  (Ouv- 
rard, C.  R.  117.  107.) 

As2SI4.    (Ouvrard.) 

See  also  Arsenyl  sulphoiodide. 

Arsenic  sulphoselenide,  As2SeS2. 

Easily  sol.  in  cold  NH4SH+Aq.  Nearly 
completely  sol.  in  (NH4)2CO3+ Aq.  (v.  Ge- 
richten,  B.  7.  29.) 

As2SSe2.  More  difficultly  sol.  than  the  pre- 
ceding comp.  in  NH4SH+Aq.  (v.  Gerichten.) 

As2Se2S3.    Sp.  gr.  =  6.402  at  ca.  750°. 

Insol.  in  most  solvents.  Easily  sol.  in  al- 
kali hydroxides  and  sulphides +Aq.  (Szar- 
vasy,  B.  1895,  28.  2661.) 

As2Se3S2.    Sp.  gr.  =  11.35  at  550-600°. 

Insol.  in  most  solvents.  Easily  sol.  in 
alkali  hydroxides  and  sulphides +Aq.  (Szar- 
vasy,  B.  1895,  28.  2659.) 

Arsenic  telluride,  As2Te2. 

Sol.  in  HNO3  and  HNO3+HCl+Aq.  (Op- 
penheim,  J.  pr.  71.  266.) 

As2Te3.    As  above.    (Oppenheim.) 

Arsenic  acid,  anhydrous,  AsaOs. 
See  Arsenic  pentoxide. 

Metaarsemc  acid,  HAsO3. 

Slowly  sol.  in  cold,  quite  easily  sol.  in  hot 
H2O,  with  considerable  evolution  of  heat, 
and  conversion  into  H3AsO4.  (Kopp,  A.  ch. 
(3)  48.  196.) 

OrthoSLTsemc  acid,  H3As04. 

Sol.  in  H2O,  with  absorption  of  heat. 

1  pt.  As2O5  dissolves  in  0.405  pt.  H2O  at 


pts. 


pt.  1 

12.5°,  or  100  pts.  H2O  dissolve  244.81 
As205  at  12.5°.    (Vogel.) 

Sol.  in  0.5  pt.  H2O.    (Thenard.) 

Sol.  in  6  pts.  cold  H2O,  and  more  quickly  in 
2  pts.  hot  H2O.    (Bucholz.) 

100  pts.  H2O  at  15.56°  dissolve  150  pts. 
As2O6.    (lire's  Diet.) 

H3AsO4+Aq   sat.    at    15°    contains    15% 
As2O5. 

Sp.  gr.  of  H3As04+Aq  at  15°:  a  =  sp.  gr.  if 
%  is  As2O5;  b  =  sp.  gr.  if  %  is  H3AsO4. 


% 

a 

6 

% 

a 

b 

5 
10 
15 
20 
25 
30 
35 
40 

1.042 
1.085 
1.134 
1.187 
1.245 
1.306 
1.378 
1.453 

1.0337 
1.0690 
1.1061 
1.1457 
1.1882 
1.2342 
1.2840 
1.3382 

45 
50 
55 
60 
65 
70 
75 

1.540 
1.635 
1.742 

1.3973 
1.4617 
1.5320 
1.6086 
1.6919 
1.7827 

(Schiff,  A.  113.  183,  calculated  by  Gerlach, 
Z.  anal.  27.  303.) 

60 


ARSENIC  .ACID 


Sp.  gr.  of  H3AsO4+Aq  at  15°:  a  =sp.  gr.  if  % 
is  As2O5;  6  =  sp.  gr.  if  %  is  H3AsO4. 

less  sol.  in  HC2H3O2+Aq.     The  neutral  al- 
kaline-earth arsenates  are  less  sol.  in  NH4OH 

I    A  /-*  -fVioTi  in  TT«r^    Viiii"  mnvp  Qnl     "in   "NTTTjf^l- 

% 

a 

b 

% 

a 

b 

^^.fV(_|   Tjlldll  ill  XI  2^-';    LHIL  lil<Jl  "  oUl.   Ill   J-i  J-J-4^-/l    |^ 

Aq  (Field).    The  alkali  arsenates  are  sol.  in 

i      .      i           •             /T     p\  -«rt    f~^    T)     1  AO     i  r\co  \ 

11 

hot  glycerine.     (Leievre,  O.  K.  108.  1058.) 

1 

1.008 

1.006 

47 

1.564 

1.412 

2 

1.016 

1.013 

48 

1  .  582 

1.425 

Aluminum  arsenate,  Al2(AsO4)2. 

3 
4 
5 
6 

1.023 
1.031 
1.039 
1.048 

1.019 
1  026 
1.032 
1.039 

49 
50 
51 
52 

1.601 
1.620 
1.642 
1.663 

1.437 

1.'464 
1.478 

Ppt.    Insol.  in  H2O;  difficultly  sol.  in  acids. 
(Coloriano,  C.  R.  103.  273.) 
Insol.  in  acetone.    (Naumann,  B.  1904,  37. 

7 
8 
9 

1.057 
1.065 
1.074 

1.046 
1.052 
1.059 

53 
54 
55 

1.685 
1.706 
1.728 

1.49i 
1.505 
1.519 

2A12O3,    3As2O5.      Nearly   unattacked  by 
boiling  H2O;  sol.  in  dil.  acids.     (Lefevre,  A. 
rh    (ft}  27    ^  } 

10 

1.083 

1.066 

56 

1.752 

1.534 

1>U«    \\J  J    At*   *J  •  J 

11 
12 

1.092 
1.102 

1.073 
1.081 

57 

58 

1.777 
1.801 

1  549 
1.564 

Aluminum  potassium  arsenate,  2A12O3,  3K20, 

13 

1.111 

1.088 

59 

1.825 

1.579 

0     2    5-                                          " 

14 

1.121 

1.096 

60 

1.850 

1.594 

(Lefe"vre.) 

15 

1  130 

1  103 

61 

1.880 

1      A1  ft 

16 

l!l40 

1.111 

62 

1.910 

1.'626 

Aluminum  sodium  arsenate,  2A12O3,  3Na2O, 

17 

1.150 

1.119 

63 

1.940 

1.643 

3As2O5. 

18 

1.160 

1.126 

64 

1.970 

1.659 

(Lefevre.) 

19 

1.170 

1.134 

65 

2.000 

1.675 

20 

1.180 

1.142 

66 

2.030 

1.693 

Ammonium  arsenate,  (NH4)3AsO4+3H2O. 

21 

1.191 

1.150 

67 

2.060 

1.71o 

Difficultly  sol.  in  H2O.    Less  sol.  in  H2O 

22 

1.203 

1.158 

68 

2.090 

1  73o 

than  (NH4)2HAsO4.    (Mitscherlich.) 

23 

1.214 

1.167 

69 

2.120 

1.749 

Insol.  in  liquid  NH3.    (Franklin,  Am.  Ch. 

24 

1.226 

1.175 

70 

2.150 

1.767 

J.  1898,  20.  826.) 

25 

1.237 

1.183 

71 

l-78g 

26 

1.249 

1.192 

72 

1.809 

Ammonium  hydrogen  arsenate, 

27 

1.261 

1.201 

73 

1.830 

(NH4)2HAs04. 

28 
29 
30 

1.274 
1.286 
1.298 

1.210 
1.219 

1  228 

74 
75 
76 

1.85i 
1.872 

1  897 

Effloresces,  giving  off  NH3;  more  sol.  in 
H2O  than  (NH4)3AsO4.     (Salkowsky,  J.  pr. 

•4  f\Jt          -I  f\{\     \ 

31 
32 

1.312 
1.325 

1.238 
1.248 

77 
78 



1.92i 
1.946 

104.  129.) 
Insol.  in  acetone.     (Eidmann,  C.  C.  1899, 

33 

1.339 

1.257 

79 

1.97n 

'^ 

34 
35 
36 
37 

1.352 
1.366 
1.381 
1.396 

1.267 
1.277 

1.288 
1.299 

80 
81 
82 
83 

u 

1.995 

2.020 
2.045 
2.070 

Ammonium  ^"hydrogen  arsenate, 
NH4H2As04. 
Not  efflorescent.    Very  sol.  in  H20. 

38 

1.411 

1.309 

84 

2  095 

39 

1.426 

1.320 

85 

2.'l20 

Ammonium  barium  arsenate,  NH4BaAsO4  + 

40 

1.441 

1.331 

86 

2.149 

J^H^. 

41 
42 

1.458 
1.475 

1.342 
1.353 

87 
88 

2.178 
2.207 

Sol.  by  10  days'  contact  in  1391  pts.  H2O; 
m  18,832  pts.  of  a  mixture  of  1  pt.  NH4OH  + 

43 

1.492 

1.366 

89 

2.236 

Aq  and  3  pts.  H2O;  in  227  pts.  of  a  solution 

44 

1.509 

1.376 

90 

2.265 

of  1  pt.  NH4C1  in  10  pts.  H2O;  and  in  2169 

45 

1.526 

1.387 

91 

2.295 

)ts.  of  a  solution  of  1  pt.  NH4C1  in  10  pts. 

46 

1.545 

1.400 

NH4OH+  Aq  and  60  pts.  H2O.     (Lefevre, 

A        s\V\       1  Of\O       /£!\    rtfT      1  O    \ 

(Kopp,  calculated  by  Gerlach,  Z.  anal.  27. 

A.  cn.  189J,  (b)  27.  13.) 
(NH4)2BaH2(AsO4)2.    Efflorescent.     Insol. 

316.) 
See  also  Arsenic  pentoxide. 

n  H20;  easily  sol.  in  dil.  HN03+Aq.    (Bau- 
mann,  Arch.  Pharm.  36.  36.) 

P«/roarsenic  acid, 

Very  deliquescent;  easily  sol.  in  H20  with 
evolution  of  much  heat,  and  conversion  into 
H3As04. 

Arsenates. 

Arsenates  of  the  alkali  metals,  and  acid 
arsenates  of  the  alkaline-earth  metals  are  sol. 
in  H2O.  Neutral  and  basic  arsenates  are 
easily  sol.  in  mineral  acids,  including  H3AsO4; 


Ammonium  calcium  arsenate,  NH4CaAsO4+ 


1000  pts.  pure  H2O  dissolve  0.20  pt.  this 
alt;  1000  pts.  NH4Cl+Aq  (containing  50  pts. 

NH4C1)  dissolve  4.15  pts.  this  salt;  900  pts. 

H2O  +  100pts.  NH4OH  (sp.  gr.  =0.880)  dis- 
olve  0.01  pt.  this  salt.  (Field,  Chem.  Soc.  11. 

Soluble  by  10  days'  contact  in  2167  pts.  H2O 
at  15°;  in  381  pts.  NH4Cl+Aq  (1  :7);  in 


ARSENATE  TELLURATE,  AMMONIUM 


61 


43478  pts.  NH4OH+Aq  (1  :  3);  in  10570  pts. 
NH4Cl+NH4OH+Aq  (1  :  10  :  60).  (Lefevre, 
A.  ch.  1892,  (6)  27.  13.) 

+6H2O.  Sol.  in  hot,  very  si.  sol.  in  cold 
H2O;  si.  sol.  in  NH4C1,  and  NH4OH+Aq 
(Wach,  Schw.  J.  12.  285.) 

+7H2O.    (Bloxam,  C.  N.  54.  163.) 

(NH4)2CaH2(AsO4)2.  Efflorescent.  Insol. 
in  H2O;  easily  sol.  in  dil.  HNO3+Aq.  (Bau- 
mann,  Arch.  Pharm.  36.  36.) 

(NH4)Ca3H2(AsO4)3+3H2O. 

(NH4)Ca6H5(AsO4)6+3H2O.  (Bloxam,  C. 
N.  54.  163.) 

Ammonium  glucinum  arsenate,  NH4GlAsO4 


More  stable  than  the  corresponding  potas- 
sium salt.  (Bleyer,  Z.  anorg.  1912,  75.  291.) 

Ammonium  iron  (ferric)  dihydrogen  arsenate. 
NH4H2AsO4,  FeAsO4. 

Hydrolyzed  by  H2O. 

Sol.  in  cold  cone.  HC1,  hot  HNO3,  hot  dil. 
H2SO4,  and  in  hot  arsenic  acid+Aq  contain- 
ing 75%  arsenic  pentoxide. 

Sol.  in  hot  cone.  NH4OH+Aq.  Completely 
hydrolyzed  by  caustic  alkalies. 

Insol.  in  cone.  NH4Cl+Aq  and  in  50% 
acetic  acid.  (Curtman,  J.  Am.  Chem.  Soc. 
1910,  32.  628.) 


lesium  arsenate, 


Ammonium  maj 
NH4MgAs4. 

SI.  sol.  in  H2O.    Sol.  in  acids. 

Anhydrous  salt  is  sol.  in  2784  pts.  H2O  at 
15°;  in  15,904  pts.  NH4OH+  Aq  (1  :  3)  (0.96 
sp.  gr.);  in  1386  pts.  NH4Cl+Aq  (1  :  70);  in 
886.7  pts.  NH4Cl+Aq  (1  :7);  in  3014  pts. 
NH4C1  (1  pt.)+NH4OH  (0.96  sp.  gr.)  (10 
pts.)+Aq  (60  pts.);  in  32,827  pts.  magnesia 
mixture.  (Fresenius,  Z.  anal.  3.  206.) 

Anhydrous  salt  is  sol.  in  4389  pts.  NH4NO3 
+Aq  (1  :50);  in  2561.5  pts.  KCl+Aq  (1  : 
165);  in  1422  pts.  ammoniacal  solution  of  3.5 
g.  tartaric  acid  in  250  cc.  H2O;  in  933.5  pts. 
ammoniacal  solution  of  2.5  g.  citric  acid  in 
250  cc.  H2O.  (Puller,  Z.  anal.  10.  62.) 


Sol.  in  2656  pts.  H2O  at  15°;  in  15,038  pts. 
NH4OH+Aq  (1  :  3)  (0.96  sp.  gr.);  in  844  pts. 
NH4Cl+Aq  (1:7);  in  1315  pts.  NH4Cl+Aq 
(1  :  70);  in  2871  pts.  NH4C1  (1  pt.)+NH4OH 
(0.96  sp.  gr.)  (10  pts.)+Aq  (60  pts.).  (Fre- 
senius.) 

1000  pts.  pure  H2O  dissolve  0.14  pt.  salt; 
1000  pts.  NH4Cl+Aq  (containing  100  pts. 
NH4C1)  dissolve  0.95  pt.  salt;  900  pts.  H2O 
+  100  pts.  NH4OH  (sp.  gr.  0.880)  dissolve 
0.07  pt.  salt.  (Field,  Chem.  Soc.  11.  6.) 

+6H2O.  SI.  efflorescent.  SI.  sol.  in  H,O. 
Very  si.  sol.  in  NH4OH+Aq. 


Solubility  of  NH4MgAsO4+6H2O  in  H2O  and  NH4  salts +Aq. 
Grams  salt  dissolved  in  100  g.  solvent. 


t° 

H2O 

5% 
NH4NOa+Aq 

5% 
NH4Cl+Aq 

NH4OH-t-Aq 
1  pt.  NH4OH  + 
Aq  (0.96)  +4  pts. 
H2O 

4%  NEUOH  + 
Aq+5% 
NH4Cl+Aq 

4%  NH4OH  + 
Aq  +10% 
NH4Cl+Aq 

0° 

0.03388 

0.09216 

0.08397 

0.00874 

20 
30 

0.02066 

0.11358 
0  11758 

0.  12284 
0  11204 

0.00958 

0.01331 

0.03165 

40 

0  02746 

0  13936 

0  19016 

0  01173 

50 

0.02^61 

0  18945 

0  18889 

0.01005 

60 
70 

•  0.02103 
0.01564 

0.21115 
0  18880 

0.21952 
0  22092 

0.00902 
0.00949 

0.04691 

0.05353 

80 

0.02364 

0.  18945 

0.23144 

0.00912 

(Wenger,  Dissert.  1911.) 


Ammonium   manganous    arsenate, 

NH4MnAsO4+6H2O. 

Nearly  insol.  in  cold  H2O;  easily  sol.  in  dil. 
acids;  insol.  in  alcohol.    (Otto,  J.  pr.  2.  414.) 

Ammonium  sodium  arsenate.  NH4NaHAsO4 

+4H20. 

Sol.  in  H2O.     (Uelsmann,  Zeit.  f.  ges.  Nat. 
23.  347.) 

Ammonium   sodium  hydrogen   arsenate, 

(NH4)3Na3H6(AsO4)4+6H2O. 
Sol.  in  H2O.     (Filhol  and  Senderens,  C.  R. 
94.  649.) 

Ammonium  strontium  arsenate,  NH4SrAsO4 


. 

Sol.  by  10  days'  contact  in  3229  pts.  H2O, 
in  11,586  pts.  dil.  NH4OH+Aq,  in  199  pts. 


of  a  mixture  of  1  pt.  NH4C1  in  7  pts.  H2O, 
and  in  1519  pts.  of  a  solution  of  1  pt.  NH4C1 
in  10  pts.  NH4OH+Aq  and  60  pts.  HoO. 
(Lefevre,  A.  ch.  1892,  (6)  27.  13.) 

Ammonium  uranyl  arsenate,  NH4(UO2)AsO4 


Insol.  in  H2O,  HC2H3O2,  and  saline  solu- 
tions as  NH4Cl+Aq;  sol.  in  mineral  acids. 
(Puller,  Z.  anal.  10.  72.) 

Ammonium  vanadium  arsenate, 

NH4(V02)2As04,    and    (NH4)2HAsO4+ 
2(VO2)2H2AsO4. 
See  Arseniovanadate,  ammonium. 

Ammonium  arsenate  tellurate.  • 
See  Arseniotellurate,  ammonium. 


62 


ARSENATE,  ANTIMONY 


Antimony  arsenate  (?). 

Insol.  in  H20;  insol.  in  acids  after  ignition, 
but  when  fresh  is  sol.  in  cone,  boiling  HC1+ 
Aq,  and  si.  sol.  in  HNO3+Aq.  (Dumas.) 

Barium  arsenate,  Ba3(AsO4)2. 

1000  pts.  pure  H2O  dissolve  0.55  pt. 
Ba3(AsO4)2;  1000  pts.  NH4Cl+Aq  (containing 
50  pts.  NH4C1)  dissolve  1.95  pts.  Ba3(AsO4)2; 
900  pts.  HoO  +  100  pts.  NH4OH+Aq  (sp.  gr. 
=  0.88)  dissolve  0.03  pt.  Ba3(AsO4)2.  (Field, 
Chem.  Soc.  11.  6.) 

Sol.  in  cold  HNO3,  and  HCl+Aq  (Berze- 
lius);  H2C4H406,  and  HC2H302+Aq.  (An- 
thon.) 

Solubility  in  H2O  is  not  increased  by  pres- 
ence of  NH4,  Na,  or  K  salts.  (Laugier.) 

Not  pptd.  in  presence  of  Na  citrate. 
(Spiller.) 

.    (Salkowsky,  J.  pr.  104.  129.) 


Barium     hydrogen     arsenate,     BaHAsO4+ 


. 

Very  si.  sol.  in  H2O,  but  decomp.  thereby 
into  Ba3(As04)2  and  BaH4(AsO4)2.  (Berze- 
lius.) 

SI.  sol.  in  cold  acids. 

+H2O.  SI.  sol.  in  either  BaCl2+Aq  or 
Na2HAsO4+Aq.  (Maumene,  J.  B.  1864. 
237.) 

Barium  tetrahyfaogen  arsenate,  BaH4(AsO4)2 
+2H20. 

Easily  sol.  in  H2O.  (Setterberg,  Berz.  J.  B. 
26.  206.) 

Difficultly  sol.  in  little,  but  decomp.  by  much 
H2O.  Easily  sol  in  'HCl+Aq,  less  easily  in 
HC2H302+Aq  (Hermann,  Dissert,  1879.) 

Barium  arsenate,  acid,  BaO,  2As2O5+4H2O. 
Very  si.  sol.  in  H2O.    (Mitscherlich.) 

Barium  p?/roarsenate,  Ba2As207. 

Insol.  in  H2O,  but  decomp.  thereby  into 
BaHAsO4-f  H2O.  (Lefevre,  C.  R.  108/1058.) 

Barium  potassium  arsenate,  BaKAsO4. 

SI.  decomp.  by  cold  H2O;  rapidly  sol.  in 
dil.  acids.  (Lefevre,  A.  ch.  (6)  27.  1.) 

Barium  sodium  arsenate,  BaNaAsO4+ 
(Joly,  C.  R.  1887,  104.  1702.) 

Barium  arsenate  chloride,  3Ba3(AsO4)2,  BaCl2. 
Insol.    in   H20;   sol.    in  .dil.    HNO3-f  Aq. 
(Lechartier,  C.  R.  65.  172.) 

Bismuth  arsenate,  basic,  BiAsO4,  3Bi2O3. 
Insol.    in    H2O.      Sol.    in    mineral    acids. 

(Cavazzi,  Gazz.  ch.  it.  14.  289  ) 
5Bi2O3,  2As2O5+8H2O.    Min.  Rhagite 
Easily  sol.  in  HCl+Aq;  si.  sol.  in  HN03+ 

Aq. 


Bismuth  arsenate, 

Insol.  in  H2O.     Insol.  in  HNO3+Aq  in 

presence  of  H3AsO4,  or  alkali  arsenates+Aq; 

sol.  in  HCl+Aq.     (Salkowsky,  J.  pr.  104. 

129.) 
Not      wholly      insol.      in      HNO3+Aq. 

(Schneider,  J.  pr.  (2)  20.  418.) 
Very  sol.  in  H3AsO4+Aq.    (Dumas.) 
Insol.  in  Bi(NO3)3+Aq.    (Dumas.) 
Sol.  in  Bi(NO3)3+Aq.    (Salkowsky.) 
Insol.  in  cone.  Bi(NO3)3+Aq  containing  a 

small  quantity  of  HNO3.    (Schneider.) 

Bismuth  copper  arsenate,  BioCu2oAs:oH4407o 

=  Bi2O3,  20CuO,  5As2O5+22H2O. 
Min.  Mixite.    Decomp.  by  dil.  HNO3+Aq 
into  insol.  BiAsO4,  and  Cu3(AsO4)2,  which 
goes  into  solution.    (Dana.) 

Bismuth  uranyl  arsenate,  Bi2(As04)2, 

8BiO3H3,  (UO2)3(AsO4)2. 
Min.  Walpurgite. 

Cadmium  arsenate,  Cd3(AsO4)2. 
Ppt.    (Salkowsky,  J.  pr.  104.  129.) 
2CdO,  As2O5.    (Lefevre,  C.  R.  110.  405.) 
5CdO,  2As2O5+5H2O.    Ppt,    (Salkowsky.) 

Ca\imium  p?/r0arsenate,  Cd2As2O7. 
(de  Schulten.) 

Cadmium   hydrogen   arsenate,    CdHAsO4+ 

H2O. 

Decomp.  by  H2O.    (Demel,  B.  12.  1279.) 
CdH4(AsO4)2+2H2O.    Decomp.  by  excess 

of  H2O.    (de  Schulten,  Bull.  Soc.  (3)  1.  473.) 

Cadmium  potassium  arsenate,  2CdO,  K20, 

As2O5. 
(Lefevre,  C.  R.  110.  405.) 

Cadmium  sodium  arsenate,  CdO,  2Na20, 
As2O5. 

Slowly  sol.  in  dil.  acids.  (Lefevre,  C.  R. 
110.  405.) 

2CdO,  4Na2O,  3As2O6.    (Lefevre.) 

Cadmium    arsenate    bromide,    3Cd3(AsO4)2, 

CdBr2. 

Sol.  in  very  dil.  HNO3+Aq.  (de  Schulten, 
Bull.  Soc.  (3)  1.  472.) 

Cadmium  arsenate  chloride,  3Cd3(AsO4)2, 
CdCl2. 

Sol.  in  very  dil.  HNO3+Aq.    (de  Schulten.) 

Caesium  arsenate,  Cs2O,  2As2O5+5H2O. 

Ppt.    (Ephraim,  Z.  anorg.  1910,  65.  246.) 
Calcium  arsenate,  Ca3(AsO4)2+3H2O. 

Ppt.  Insol.  in  H2O;  sol.  in  H3AsO4+Aq. 
(Kotschoubey,  J.  pr.  49.  182.) 

Calcium  p?/roarsenate,  Ca2As2O7. 

Slowly  decomp.  by  cold  H2O  into  CaHAsO4 
.    (Lefevre.) 


ARSENATE,  BASIC,  CUPRIC 


63 


Calcium  hydrogen  arsenate,  CaHAsO4+ 
^H20. 

Insol.  in  H2O.    (Debray,  A.  ch.  (3)  61.  419.) 

+H2O.  Min.  Haidingerite.  Easily  sol.  in 
acids. 

+2;HjH2O.  Nlui^Pharmacolite.  Easily  sol. 
in  acids. 

+3H2O.  Insol.  in  H,O ;  sol.  in  HC1,  HNO3, 
or  H3AsO4+Aq;  also  in  (NH4)2S04,  NH4NO8, 
NH4C2H3O2,  and  NH4Cl-fAq.  (Pfaff.) 

Calcium  teJrahydrogen  arsenate, 

CaH4(AsO4)2. 

Sol.  inH2O.    (Graham.) 

+H2O.  SI.  sol.  in  H2O.  Decomp.  by 
much  hot  H2O  into  H3AsO4  and  Ca3(AsO4)2. 
(Hermann,  Dissert.  1879.) 

Calcium  iron  (ferric)  arsenate,  6CaO,  4Fe2O3, 

5As2O5  +  15H2O  (?). 
Min.  Arseniosiderite.    Sol.  in  acids. 

Calcium  magnesium  arsenate,  Ca5H2(AsO4)4, 
Mg5H2(AsO4)4  +  10H2O. 

Min.  Picropharmacolite.  Easily  sol.  in 
acids. 

Ca3(AsO4)2,  Mg3(As04)2.  Sol.  in  HNO3  + 
Aq.  (Kiihn.) 

Min.  Berzeliite.    Sol.  in  HNO8+Aq. 

Ca8Mg6Hi4(AsO4)i4+49H2O.  Min.  Wap- 
plerite. 

Calcium  potassium  arsenate,  CaKAs04. 

(Lefevre,  A.  ch.  (6)  27.  5.) 
Calcium  sodium  arsenate,  CaNaAsO4. 

(Lefevre,  A.  ch.  (6)  27.  1.) 

4CaO,  2Na2O,  3As2O5.  Not  attacked  by 
boiling  H2O;  easily  sol.  in  dil.  acids,  (Le- 
fevre.) 

Calcium  uranyl  arsenate,  Ca(UO2)2(AsO4)2+ 

8H2O. 
Min.  Uranospinite. 

Calcium     vanadium     arsenate,     CaHAs04, 

2(VO2)H2AsO4+8H2O. 
See  Arseniovanadate,  calcium. 

Calcium  arsenate  chloride,  Ca3(As04)2,  CaCl2 
Insol.    in   H2O;    sol.    in   dil.    HNO3+Aq 
(Lechartier.  C.  R.  65.  172.) 

3Ca3(AsO4)2,  CaCl2.  As  above.  (Le- 
chartier.) 

Cerous  arsenate,  CeHAsO4. 

Insol.  in  H2O.  Sol.  in  arsenic  acid+Aq 
(Berzelius.) 

Ceric    hydrogen     arsenate,     Ce(HAs04)2+ 

6H2O. 

Ppt.  Insol.  in  H2O  and  dil.  acids.  (Bar 
bieri,  B.  1910,  43.  2216.) 

Ceric  cfthydrogen  arsenate.   Ce(H2AsO4)4+ 

4H20. 
Sol.  in  cone.  HNO3.     (Barbieri  I.  c.) 


Chromic  arsenate,  2Cr2O3,  3As2O5. 

Insol.  in  H2O  and  cone,  boiling  acids.  (Le- 
evre,  A.  ch.  (6)  27.  5.) 

!hromic  potassium  arsenate,  2Cr2O3,  3K2O, 
3As2O5. 

(Lefevre.) 

Chromic  sodium  arsenate,  2Cr2O3,  3Na2O, 
3As2O5. 

(Lefevre.) 
Cobaltous  arsenate,  basic,  4CoO,  As2O5. 

Easily  sol.  in  acids.  (Gentele,  J.  B.  1851. 
559.) 

Co(CoOH)AsO4.  Insol.  in  H2O;  difficultly 
sol.  in  acids.  (Coloriano.) 

Cobaltous  arsenate,  Co3(AsO4)2+8H2O. 

Ppt.  Insol.  even  in  boiling  H2O;  easilv 
sol.  in  HNO3,  HC1,  and  NH4OH+Aq;  sol.  in 
H3As04+Aq  (Proust);  sol.  in  dil.  FeSO4+Aq. 
Karsten,  Pogg.  60.  266.) 

Min.  Cobalt  bloom.  Erythrite.  Easily  sol.  in 
acids. 

5CoO,  2As2O5+3H2O.  Insol.  in  H2O;  dif- 
ficultly sol.  in  acids.  (Coloriano,  C.  R.  103. 
273.) 

2CoO,  AsaOs.  SI.  attacked  by  boiling  H2O; 
easily  sol.  in  dil.  acids.  (Lefevre.) 

Cobaltous  hydrogen  arsenate,  CoH4(AsO4)2. 
Sol.  in  H20. 

Cobaltous  potassium  arsenate,  CoKAsO4. 

(Lefevre.) 

Cobaltous  sodium  arsenate,  CoNaAsO4. 

(Lefevre.) 

4CoO,  2Na2O,  3As2O5.    (Lefevre.) 

Cobaltous  vanadium  arsenate, 

Co(V02)2H2(As04)2+8H20. 
See  Arseniovanadate,  cobaltous. 

Cobaltous    arsenate    ammonia,    Co3(AsO4)2, 

NH3+7H2O. 

(Ducru,  A.  ch.  1901,  (7)  22.  185.) 
Co3(AsO4)2,  2NH3+6H2O.    (Ducru,  I  c.) 
Co3(AsO4)2,  3NH3+5H2O.    (Ducru,  I,  c.) 

Cuprous  arsenate,  2Cu2O,  As2O5. 
(Hampe,  Dissert.  1874.) 
4Cu2O,  As2O6.    (Hampe,  L  c.) 

Cuprous  p^/roarsenate,  Cu4As2O7. 

Ppt.  Sol.  in  NH4OH  or  KOH+Aq. 
(Reichard,  B.  1898,  31.  2166.) 

Cupric  arsenate,  basic,  8CuO,  As2O5-f 
12H2O. 

Min.  Chalcophyllite.  Easily  sol.  in  acids 
andNH4OH+Aq. 

6CuO,  As2O5+3H2O.  Min.  Aphanesite, 
Clioclasite.  Sol.  in  acids  and  ammonia. 

5CuO,  As2O5+2H2O.  Min.  Erinite.  Sol. 
in  HNOs+Aq. 


64 


ARSENATE,  CUPRIC 


+5H2O.  Min.  Cornwallite.  Sol.  in  acids, 
andNH4OH+Aq. 

+9H2O.     Min.  Tirolite. 

4CuO,  As2O5+H2O.  Insol.  in  H2O.  (De- 
bray,  A.  ch.  (3)  61.  423.) 

Min.  Olivenite.  Sol.  in  acids,  and  NH4OH 
+Aq;  decomp.  by  hot  KOH+Aq. 

+7H2O.  Min.  Euchrvite.  Sol.inHNO3  + 
Aq. 

+4^H2O.    (Hirsch,  C.  C.  1891,  I.  15.) 

Cupric  arsenate,  Cu3(AsO4)2. 

Insol.  in  H2O.  Easily  sol.  in  HCl+Aq;  si. 
sol.  in  other  acids;  sol.  in  NH4OH+Aq. 
(Coloriano,  C.  R.  103.  273.) 


Insol.  in  methyl  acetate. 
1909,  42.  3790.) 


(Naumann,  B. 


Insol.  in  liquid  NH3.     (Franklin,  Am.  Ch. 

J.  1898,  20.  827.) 

+4H2O.    Decomp.  by  hot  H2O.    (Debray.) 
+5HoO.     Min.  Trichalcite.     Easily  sol.  in 

cold  HCl+Aq. 

Cupric  arsenate,  acid,  5CuO,  2As2O5. 

Sol.  in  H2SO3+Aq.    (Vogel.) 

+3H2O.    (Salkowsky.) 

+8,  9M,  and  12HH2O.     (Hirsch.) 

CuHAsO4+H2O.  Insol.  in  H20.  (Color- 
iano.) 

+  1^H2O.  Insol.  in  H2O.  (Debray,  A. 
ch.  (3)  61.  419.) 

8CuO,  3As2O5+12H2O.    (Hirsch.) 

Cupric  lead  arsenate,  3CuO,  PbO,  As2O5+ 
2H2O. 

M  in .  Bayldonite .  Nearly  insol .  in  HNO  3 + 
Aq. 

Cupric  potassium  arsenate,  CuKAs04. 

Slowly  sol.  in  NH4OH+Aq;  easily  sol.  in 
acids.  (Lefevre,  A.  ch.  (6)  27.  5.) 

8CuO,  K2O,  As2O6.  Easily  sol.  in  dil.  acids. 
(Lefevre.) 

Cupric  sodium  arsenate,  CuNaAs04. 

(Lefevre.) 

3CuO,  Na2O,  2As2O5.  Very  sol.  in  dil. 
acids.  (Lefevre.) 

2Cu3(AsO4)2,  NaH2AsO4+5H2O.  Ppt. 
(Hirsch,  C.  C.  1891,  I.  15.) 

6Cu3(AsO4)2,  2NaH2As04,  Na2HAsO4+ 
13y2  H2O,  or  16H2O.  Ppt.  (Hirsch.) 

3Cu3(AsO4)2,   Na2HAsO4+9^H2O.     Ppt. 


(Hirsch.) 

4Cu3(AsO4)2,    Na2HAs04+llH2O. 
(Hirsch.) 


Ppt. 


Cupric  uranyl  arsenate,  Cu(UO2)2(AsO4)2  + 
8H2O. 

(Wither,  A.  68.  312.) 
Min.  Zeunerite. 

Cupric  vanadium  arsenate, 

Cu(V02)2H2(As04)2+3H20. 
See  Arseniovanadate,  cupric. 


Cupric  arsenate  ammonia,  Cu3(AsO4)2, 
3NH3+4H2O. 

Insol.  in  cold  or  hot  H2O.  (Damour,  J.  pr. 
37.  485.) 

2CuO,  As2O5,  4NH3+3H20.  Decomp.  by" 
H2O.  (Schiff,  A.  123.  42.), 

Cupric  arsenate  calcium  carbonate,  5CuO, 

As2O5,  CaCO3+4H2O,  or  9H2O. 
Min.  Tyrolite.      Easily  sol.  in  acids,  and 
NH4OH+Aq. 

Cupric  arsenate  sodium  chloride.  2Cu3(AsO4)->, 

NaCl+7^H20. 

Decomp.  by  hot  H2O.  (Hirsch,  Dissert. 
1891.) 

3Cu3(As04)2,  2NaCl  +  13^H2O. 
+  17^H2O.    (Hirsch,  i.e.) 
5Cu3(AsO4)2,  3NaCl+23H20.    (Hirsch.) 

Didymium  arsenate,  Di2H3(As04)3. 

Ppt.  Insol.  in  H2O;  si.  sol.  in  weak  acids. 
(Marignac,  A.  ch.  (3)  38.  164.) 

5Di2(AsO4)2,  As2O6+3H20.    Ppt. 

Glucinum  arsenate,  Gl3(AsO4)2. 

Insol.  in  H2O;  sol.  in  H3As04+Aq.     (Ber- 

zelius.) 

Glucinum  hydrogen  arsenate,  GlHAs04. 

Obtained  in  impure  state  by  heating  As2O6 
with  G1(OH)2  in  a  sealed  tube  at  220°. 
(Bleyer,  Z.  anorg.  1912,  76.  287.) 

Glucinum  Ze/rahydrogen  arsenate, 

GlH4(As04)2. 

Very  hydroscopic.  (Bleyer,  Z.  anorg.  1912, 
75.  287.) 

Glucinum    potassium    arsenate.    KGlAsO4, 

HG1O+5H2O. 

Unstable.  Amorphous.  Easily  hydrolyzed, 
giving  more  basic  salts.  (Bleyer,  Z.  anorg. 
1912,  76.  289.) 

Glucinum      sodium     arsenate,     NaGlAsO4. 


Unstable.  Easily  hydrolyzed.  (Bleyer, 
Z.  anorg.  1912,  75.  290.) 

Iron      (ferrous)      arsenate,      Fe3(AsO4)2+ 
6H2O   (?). 

Ppt.  SI.  sol.  in  NH4OH+Aq.  Insol.  in 
(NH4)3As04+Aq  or  other  NH4  salts+Aq. 
(Wittstein.) 

+8H2O.  Min.  Sympksite.  Sol.  in  HC1  + 
Aq. 

Iron  (ferric)  arsenate,  basic,  16Fe203,  As2O5 
+24H2O. 

Insol.  in  NH4OH+Aq.    (Berzelius.) 

2Fe2O3,  As2O5  +  12H2O.  Insol.  in  NH4OH 
+Aq. 

3Fe2O3,  2As2O5. 

3Fe2(AsO4)2,     Fe2O6H6+12H2O.     Min. 
Pharmacosiderite.      Easily     sol.     in      acids' 
decomp.  by  KOH+Aq. 


ARSENATE,  MAGNESIUM  POTASSIUM  HYDROGEN 


65 


Iron  (ferric)  arsenate,  Fe2O3,  As2O6. 

Ppt.    Insol.  in  H2O.    Decomp.  by  hot  H2O. 

Sol.  in  HC1,  H2SO4  and  HNO3.  (Metzke, 
Z.  anorg.  1898,  19.  473.) 

+4H2O.  Min.  Scorodite.  Easily  sol.  in 
HCl+Aq;  insol.  in  HNO3+Aq. 

+8H2O.  Insol.  in  H2O.  When  freshly 
pptd.,  sol.  in  NH4OH+Aq.  Sol.  in  HC1,  or 
HNOs+Aq.  Insol.  in  HC2H302,  or  NH4 
salts +Aq.  (Wittstein.) 

Sol.  in  warm  H2SO3+Aq  or  (NH4)2SO3+ 
Aq.  (Berthier,  A.  ch.  (3)  7.  79.) 

Iron    (ferric)    arsenate,  acid,   Fe2O3,3As2O6 

+  16.7H2O. 

Ppt.;  si.  sol.  in  acids  with  a  yellow  color,  and 
in  NH4OH+Aq  with  a  red  color.  (Metzke, 
Z.  anorg.  1898,  19.  476.) 

2Fe2O 3,  3 As2O 5  +  12H2O .  Insol .  in  H2O  or 
HC2H3O2+Aq. 

Sol.  in  mineral  acids. 

Sol.  only  in  cone.  H3AsO4+Aq. 

Sol.  in  (NH4)3AsO4,  and  other  NH4  salts 
-f-Aq.    (Wittstein.) 
lol. 


+22KH20.     Ppt.     SI.  sol.  in  acids  with 
yellow  color,  and  in  NH4OH+Aq  with  a 
color.    (Metzke,  Z.  anorg.  1898,  19.  475.) 

Iron   (ferroferric)    arsenate,   6FeO,   3Fe203, 

4As2O5+32H2O. 

Insol.  in  H2O.  Sol.  in  HCl+Aq.  Decomp. 
by  KOH+Aq.  (Wittstein,  J.  B.  1866.  243.) 

Iron    (ferric)    lead    arsenate,    5Fe2(As04)2, 

Pb3(As04)2. 

Min.  Carmine  Spar.  Carminite.  Sol.  in 
acids;  KOH+Aq  dissolves  out  As2O5.  (Sand- 
berger.) 

Iron  (ferric)  potassium  arsenate,  2Fe203 , 
3K2O,  3As2O5. 

Not  attacked  by  boiling  H20;  easily  sol.  in 
dil.  acids.  (Lefevre.) 

Fe2C3,  K2O,  2As2O5.    (Lefevre.) 

Iron  (ferric)  sodium  arsenate,  Fe203,  Na2O, 

2As205. 
(Lefevre.) 
2Fe2O3,  3Na20,  3As205.  (Lefevre.) 

Lanthanum  arsenate,  La2H3(As04)3. 
(Frerichs  and  Smith.) 
Doubtful.    (Cleve,  B.  11.  910.) 

Lead  arsenate,  basic,  15PbO,2As2O6  (?). 

Ppt.  (Stromholm,  Z.  anorg.  1904,  38.  446.) 
Lead  arsenate,  Pb3(AsO4)2. 

Insol.  in  H2O,  NH4OH,  or  NH4  salts +Aq. 
(Wittstein.) 

Sol.  in  2703.5  pts.  HC2H3O2+Aq  contain- 
ing 38.94%  HC2H3O2.  (Bertrand,  Monit. 
Scient.  (3)  10.  477.) 

Sol.  in  sat.  NaCl+Aq.  (Becquerel,  C.  R. 
20.  1523.) 


Not  pptd.  in  presence  of  Na  citrate. 
(Spiller.) 

Lead  pyroarsenate,  Pb2As2O7. 

Insol.  in  H2O  or  HC2H8O2+Aq.     Sol.  in 

HC1,  or  HNOs+Aq.    (Rose.) 

Decomp.  by  cold  H20.    (Lefevre.) 
+H2O=PbHAsO4.     Ppt.     (Salkowsky,  J. 

pr.  104.  109.) 

Lead  potassium  arsenate,  PbKAsO4. 
(Lefevre,  A.  ch.  (6)  27.  5.) 

Lead  sodium  arsenate,  PbNaAsO4. 

(Lefevre.) 

4PbO,  2Na2O,  3As205.  Superficially  de- 
comp.  by  cold  H2O.  (Lefevre.) 

Lead  arsenate  chloride,  3Pb3(AsO4)2,  PbCl2. 
Sol.  in  dil.  HNO3+Aq.    (Lechartier.) 
Min.  Mimetite.    Sol.  in  HNO3,  and  KOH+ 

Aq. 

Lithium  arsenate,  Li3AsO4. 

Ppt.  Sol.  in  dil.  acids  and  in  HC2H302+. 
Aq.  (de  Schulten,  Bull.  Soc.  (3)  1.  479.) 

LiH2AsC4+3/2H2O.  Decomp.  by  H2O  into 
H3AsO4  and  Li3AsO4.  (Rammelsberg,  Pogg. 
128.  311.) 

Magnesium  arsenate,  Mg3(AsO4)2. 

Ppt. 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

+7H2O,  +8H20,  +10H20,  and  +22H20. 
(Griihl,  Dissert.  1897.) 

+8H2O.  Min.  Hvrnesite.  Insol.  in  H20; 
easily  sol.  in  acids. 

Magnesium  hydrogen  arsenate,  MgHAs04. 

+  KH2O.  Insol.  in  H2O.  (de  Schulten,  C. 
R.  100.  263.) 

+5H2O.    (Schiefer.) 

+6^H2O.  Insol.  in  H2O.  1000  pts.  boiling 
H2O  dissolve  1.5  pts.  (Thompson.) 

Sol.  in  HNO3+Aq  before  ignition,  but 
insol.  in  acids  after  ignition.  (Graham,  A.  29. 
29.) 

+7H20.  Min.  Roesslerite.  Sol.  in  HC1+ 
Aq. 

Magnesium  tefrahydrogen  arsenate, 

MgH4(As04)2. 
Very  deliquescent;  sol.  in  H2O.    (Schiefer.) 

Magnesium  potassium  arsenate,  MgKAsO4. 
Insol.  in,  but  decomp.  by  cold  H2O.  (Rose.) 
Easily  sol.  in  dil.  acids.    (Lefevre.) 
+7H2O.     (Kinkelin,  Dissert,  1893.) 
4MgO,  2K2O,  3As206.     Not  attacked  by 
boiling  H20;  slowly  sol.  in  dil.  acids.     (Le- 
fevre.) 

Magnesium   potassium  hydrogen   arsenate, 

KMgH(AsO4)2+zH2O. 
Decomp.    by    H20.      (Kinkelin,    D  ssert. 
1883.) 


66 


ARSENATE,  MAGNESIUM^POTASSIUM  SODIUM 


Mg3KH2(AsO4)3+5H2O.  (Chevron  and 
Droixhe,  J.  B.  1888,  523.) 

Magnesium    potassium    sodium    arsenate, 
Mg2KNa(As04)2+10H2O. 

(Kinkelin,  Dissert.  1883.) 
Magnesium  sodium  arsenate,  MgNaAsO4. 

Insol.  in  H20.  Very  si.  sol.  in  dil.  acids. 
(Lefevre.) 

4MgO,  2Na2O,  3As206.    (Lefevre.) 

Magnesium  vanadium  arsenate, 
MgH2(VO2)2(As04)2+9H2O  and 
MgHAsO4,  2(VO2)H2As04+9H20. 
See  Arseniovanadate,  magnesium. 

Magnesium  arsenate  chloride,  Mg3(AsO4)2, 

MgCl2. 

Insol.  in  H2O:  sol.  in  dil.  HNO3+Aq. 
•(Lechartier,  C.  R.  65.  172.) 

Magnesium  arsenate  fluoride,  Mg3(As04)2, 

MgF2. 

Insol.  in  H2O;  sol.  in  dil.  HNO3+Aq. 
(Lechartier.) 

Manganous  arsenate,  basic,  6MnO,  As2O5-f 

3H20  (?). 

Min.  Chondroarsenite.  Easily  and  com- 
pletely sol.  in  dil.  HC1,  and  HNO3+Aq. 

Manganous  arsenate,  Mn3(As04)2+H2O. 

Insol.  in  H2O;  si.  sol.  in  acids.  (Coloriano, 
C.  R.  103.  273.) 

5MnO,  2As2O6+5H2O.  Insol.  in  H20. 
(Coloriano.) 

2MnO,  As2O5.  SI.  decomp.  by  cold  H2O, 
but  rapidly  on  heating.  (Lefevre.) 

MnHAsO4+H2O.  Decomp.  by  boiling 
H2O  into  5MnO,  2As2O5+5H2O.  Sol.  in 
HNO3,  H2SO4,  or  H3AsO4+Aq. 

Manganous  £e/rahydrogen  arsenate, 

MnH4(AsO4)2. 
Deliquescent.  Easily  sol.  in  H20.  (Schiefer.) 

Manganous  potassium  arsenate,  MnKAs04. 
(Lefevre,  A.  ch.  (6)  27.  5.) 

Manganous  sodium  arsenate,  MnNaAsO4. 
Very  sol.  in  dil.  acids.    (Lefevre.) 
2MnO,  4Na2O,  3As2O5.    Not  attacked  by 

boiling  H2O;  very  sol.  in  dil.  acids.    (Lefevre.) 

Manganous  arsenate  chloride,  Mn3(AsO4)2, 

MnCl2. 

Insol.  in  H2O;  sol.  in  dil.  HNO3+Aq. 
(Lechartier,  A.  68.  259.) 

Manganic  arsenate,  Mn2(As04)2+2H2O. 

Insol.  in  H2O;  sol.  in  acids. 
Mercurous  arsenate,  (Hg2)3(AsO4)2. 

Insol.  in  H2O;  difficultly  sol.  in  acids. 
(Coloriano,  C.  R.  103.  273.)  Ppt.  (Haack, 
C.  C.  1890,  II.  736.) 


Hg2(AsO3)2.  Insol.  in  H2O,  HC2H3O2,  or 
alcohol.  Decomp.  by  cold  HCl+Aq.  SI.  sol. 
in  cold  HNO3-f  Aq,  from  which  it  is  precipi- 
tated by  NH4OH  as  Hg2HAsO4.  (Simon, 
Pogg.  41.  424.) 

Mercurous  hydrogen  arsenate,  Hg2HAsO4. 
'  Insol.  in  H20,  HC2H3O2,  or  NH4OH+Aq. 
Decomp.  by  cold  HCl+Aq;  sol.  in  cold  HNO3 
+Aq  without  decomp;  very  si.  sol.  without 
decomp.  in  NH4NO3-j-Aq.    (Simon,  Pogg.  41. 

Mercuric  arsenate,  Hg3(AsO4)2. 
•Ppt.    Sol.inH3AsO4orHNO3+Aq.  (Berg- 
man.)    Very  si.  sol.  in  H2O.    Easily  sol.  in 
HCl+Aq.    SI.  sol.  in  HNO3+Aq.    Insol.  in 
H3AsO4+Aq.    (Haack,  C.  C.  189P,  II.  736.) 

Mercurous  silver  arsenate,  Hg2AgAsO4. 

Sol.  in  hot  cone.  HNO3.  (Jacobsen,  Bull. 
Soc.  1909,  (4)  5.  948.) 

Mercurous  arsenate  nitrate,  Hg3AsO4,  HgNO3 
+H2O. 

Insol.  in  H20  or  HC2H302;  sol.  in  HNO3+ 
Aq.  (Simon,  Pogg.  41.  424.) 

3Hg3As04,2HgN03,2Hg20.  Ppt.  (Haack.) 

Molybdenum  arsenate. 

Ppt. 
Nickel  arsenate,  basic,  5NiO,  As2O5. 

Min. (Bergemann.) 

Ni(NiOH)AsO4.  Difficultly  attacked  by 
acids  or  alkalies.  (Coloriano,  Bull.  Soc.  (2) 
45.  241.) 

5NiO,  2As206+3H20.     As  above. 

Nickel  arsenate,  Ni3(AsO4)2. 

Min. (Bergemann.) 

+zH2O.  Insol.  in  H2O.  Sol.  in  H3AsO4, 
and  cone,  mineral  acids.  Easily  sol.  in 
NH4OH+Aq. 

+2H20.  Insol.  in  H20;  difficultly  sol.  in 
acids.  (Coloriano,  Bull.  Soc.  45.  241.) 

+8H2O.  Min.  Nickel-bloom,  Annabergite. 
Easily  sol.  in  acids. 

NiHAsO4+H2O.  Sol.inH2O.  Difficultly 
attacked  by  acids.  (Coloriano,  C.  R.  103. 
274.) 

Nickel  potassium  arsenate,  12NiO,  3K2O, 
5As2O5. 

(Lefevre.) 

2NiO,  K2O,  As2O5.  Rapidly  sol.  in  dil. 
acids.  (Lefevre.) 

Nickel  sodium  arsenate,  NiNaAsO4. 

Very  slowly  sol.  in  dil.  acids.    (Lefevre.) 
4NiO,  2Na2O,  3As2O5.    (Lefevre.) 

Nickel  arsenate  ammonia, 

Ni3(As04)2,NH3+7H20. 

Ni3(AsO4)2,2NH3+6H2O. 

Ni3(AsO4)2,3NH3+5H2O.  (Ducru,  C.  R. 
1900,  131.  703.) 


ARSENATE,  SODIUM 


67 


Palladium  arsenate  (?). 

Ppt. 
Platinum  arsenate  (?). 

Ppt,    Sol.  in  HNO3+Aq. 
Potassium  arsenate,  K3AsO4. 

Deliquescent.  Very  sol.  in  H2O.  (Graham, 
Pogg.  32.  47.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1904,  37.  3601.) 

Potassium  hydrogen  arsenate,  K2HAs04. 

Sol.  in  H2O. 
Potassium  efohydrogen  arsenate,  KH2AsO4. 

Sol.  in  5.3  pts.  H2O  at  6°,  forming  a  solu- 
tion of  sp.  gr.  1.1134.  Much  more  sol.  in  hot 
H20.  Insol.  in  alcohol. 

Sol.  in  26,666  pts.  boiling  cone,  alcohol.    (Wenzel.) 

Potassium  sodium  hydrogen  arsenate, 
KNaHAsO4  +  16H2O. 

Sol.  in  H20. 

K3Na3H6(As04)4+9H2O.  Sol.  in  H2O,  and 
not  easily  decomp.  thereby  into  its  constitu- 
ents. (Filhol  and  Senderens,  C.  R.  95.  343.) 

Potassium  strontium  arsenate,  KSrAsO4. 

(Lefevre,  C.  R.  108.  1058.) 
Potassium  vanadium  arsenate,  K(VO2)2As04 


See  Arseniovanadate,  potassium. 
Potassium  zinc  arsenate,  KZnAsO4. 

(Lefevre.) 
Potassium  arsenate  sulphate. 

See  Arseniosulphate,  potassium. 
Rhodium  arsenate  (?). 

Ppt. 
Rubidium  metaarsenate,  RbAsO3. 

Sol.  in  H2O.  (Bouchonnet,  C.  R.  1907, 
144.  642.) 

Rubidium  arsenate,  Rb3As04-f-2H2O. 

Very  hydroscopic;  sol.  in  H2O  to  give  an 
alkaline  solution.  Absorbs  C02  from  the  air. 
(Bouchonnet,  I.e.) 

Rubidium  pyroarsenate,  Rb4As2O7. 
(Bouchonnet,  I.e.) 

Rubidium  hydrogen  arsenate,  Rb2HAsO4+ 

+H20. 

Absorbs  CO2  from  the  air.  Very  hydro- 
scopic; sol.  in  H2O.  Insol.  in  alcohol.  (Bou- 
chonnet, I.e.) 

Rubidium  (^hydrogen  arsenate,  RbH2AsO4. 

Not  hydroscopic.  Very  sol.  in  H2O;  aq. 
solution  is  acid  to  litmus.  (Bouchonnet,  I.e.) 

Silver  arsenate,  Ag3AsO4. 

Insol.  in  H2O.  Sol.  in  acids;  easily  sol. 
in  H3AsO4+Aq.  (Joly,  C.  R.  103.  1071.) 


1 1.  H2O  dissolves  0.0085  g.  Ag3AsO4  at  20°. 
(Whitby,  Z.  anorg.  1910,  67.  108.) 

Much  less  sol.  in  H3AsO4  than  Ag3PO4. 
(Graham.) 

Sol.  in  NH4OH+Aq.    (Scheele  ) 

Sol.  in  (NHOzCOs+Aq.  Insol.  in  NH4 
sulphate,  nitrate,  or  succinate+Aq.  (Witt- 
stein.) 

Very  si.  sol.  in  NH4NO3+Aq,  more  easily 
in  HC2H3O2+Aq.  (Graham.) 

Sol.  in  Na2S2O3+Aq,  but  not  so  easily  as 
Ag3PO4. 

Not  pptd.  in  presence  of  Na  citrate. 
(Spiller.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  829.) 

Silver  hydrogen  arsenate,  Ag2HAsO4. 

Decomp.  by  H2O,  with  formation  of 
Ag3AsO4.  (Setterberg,  Berz.  J.  B.  26.  208.) 

AgH2AsO4.  Decomp.  by  H2O.  (Joly,  C. 
R.  103.  1071.) 

*Ag2O,  2As2O5.  Decomp.  by  H2O.  Rather 
si.  sol.  in  HNO3+Aq.  Very  easily  sol.  in 
NH4OH+Aq.  (Hurtzig  and  Geuther,  A. 
111.  168.) 

Silver  arsenate  ammonia,  Ag3AsO4,  4NH3. 

Easily  sol.  in  H2O.  (Widmann,  Bull.  Soc. 
(2)  20.  64.) 

Silver  arsenate  sulphate,  3Ag2O,  As2O6,  SO3. 
Decomp.    by    H2O,    with    separation    of 
Ag3As04;  decomp.  by  dil.  H2SO4+Aq.    (Set- 
terberg, Berz.  J.  B.  26.  209.) 

Sodium  arsenate,  Na3AsO4+'12H2O. 

Permanent  in  dry  air.  Sol.  in  3.57  pts.  H2O 
at  15.5°.  (Graham.)  100  pts.  H2O  at  15.5° 
dissolve  28  pts.  Na3AsO4  +  12H2O.  (Ber- 
zelius.)  Sol.  in  3.75  pts.  H2O  at  17°;  or  100 
pts.  H2O  at  17°  dissolve  26.7  pts.;  or  sat. 
Na3AsO4+Aq  at  17°  contains  21.1%  Na3AsO4 
+  12H2O  or  10.4%  Na3AsO4,  and  has  sp.  gr. 
1.1186.  (Schiff,  A.  113.  350.) 

Melts  in  crystal  H2O  at  85.5°. 

Sp.  gr.  of  Na3As04+Aq  at  17°. 


7o 


%Na3AsO4+12H2O. 


% 

Sp.  gr.. 

% 

Sp.  gr. 

% 

Sp.  gr. 

1 

2 
3 

4 
5 
6 

7 

1.0053 
1.0107 
1.0161 
1.0215 
1.0270 
1.0325 
1  .  0380 

9 
10 
11 
12 
13 
14 
15 

1.0490 
1.0547 
1.0603 
1.0659 
1.0716 
1.0773 
1  .  0830 

17 
18 
19 
20 
21 
22 

1.0945 
1  .  1003 
1.1061 
1.1121 
1.1179 
1.1238 

8 

1.0435 

16 

1.0887 

(Schiff,  calculated  by  Gerlach,  Z.  anal.  8. 286.) 

"Arseniate   of  soda"   dissolves   in   60   pts.    boiling 
alcohol.    (Wenzel.) 

+4>^H2O.    (Hall,  Chem.  Soc.  61.  93.) 
-f-10H2O.    Efflorescent.    (Hall.) 


68 


ARSENATE,  SODIUM  HYDROGEN 


Sodium    hydrogen    arsenate,    Na2HAsO4- 
7H2O. 

Not  efflorescent.    (Schiff.) 

Solubility  in  Pb(NO3)2+Aq.     A  table 
given  which  records  the  g.  of  As2O5  in  100  c 
of  the  nitrate.     (Curry,  J.  Am.  Chem.  Soc 
1915,  37.  1685.) 

+7^H2O.    (Lescoeur,  C.  R.  104.  1171.) 

+12H2O.  Efflorescent.  Sol.  in  H2O;  so 
in  1.79  pts.  H2O  at  14°;  or  100  pts.  H2O  a 
14°  dissolve  56  pts.  Na2HAsO4+12H2O.  Sat 
Na2HAsO4+Aq  contains  35.9%  Na2HAsO4+ 
12H2O,  or  16.5%  Na2HAsO4,  and  has  sp.  gr.  = 
1.1722.  (Schiff,  A.  113.  350.) 

100  pts.  H2O  at  7.2°  dissolve  22.268  pts.  (Thomp 
son.) 

100  pts.  H2O  dissolve  17.2  pts.  Na2HAsO4+ 
12H2O  at  0°,  and  140.7  pts.  at  30°.  (Tilden 
Chem.  Soc.  45.  409.) 

Melts  in  crystal  H2O  at  28°.    (Tilden.) 

Sp.  gr.  of  Na2HAsO4+Aq  at  14°. 
%  =  %Na2HAsO4+12H2O. 


% 

Sp.  gr. 

% 

Sp.  gr. 

% 

Sp.  gr. 

1 

1.0042 

15 

1.0665 

29 

1.1358 

2 

1.0084 

16 

1  .  0712 

30 

1.1410 

3 

1.0126 

17 

1  .  0759 

31 

1  .  1463 

4 

1.0168 

18 

1.0807 

32 

1.1516 

5 

1.0212 

19 

1.0855 

33 

1.1569 

6 

1.0256 

20 

1.0904 

34 

1  .  1623 

7 

1.0300 

21 

1  .  0953 

35 

1.1677 

8 

1.0344 

22 

1  .  1003 

36 

1.1731 

9 

1.0389 

23 

1  .  1052 

37 

1  .  1786 

10 

1.0434 

24 

1.1103 

38 

1.1841 

11 

1  .  0479 

25 

1.1153 

39 

1  .  1896 

12 

1.0525 

26 

1  .  1204 

40 

1  .  1952 

13 

1.0571 

27 

1.1255 

14 

1.0618 

28 

1.1306 

(Schiff,  calculated  by  Gerlach,  Z.  anal.  8. 280.) 

Insol.  in  alcohol. 

+  133^H2O.    (Setterberg.) 

Sodium  cfoliydrogen  arsenate,  NaH2AsO4  + 
H2O. 

More  sol.  in  H2O  than  Na3AsO4  or 
Na2HAsO4.  (Schiff.) 

+2H2O.  Efflorescent.  (Jolv  and  Duffet, 
C.  R.  102.  1391.) 

Sodium  frihydrogen  diarsenate, 

Na3H3(AsO4)2+3H2O. 
Sol.  in  H20.    (Filhol  and  Senderens,  C.  R. 
95.  343.) 

Sodium  strontium  arsenate,  NaSrAsO4. 
Not  attacked  by  boiling  H2O.    (Lefevre.) 
+9H2O.   Scarcely  sol.  in  H2O.    (Joly,C.R. 

104.  905.) 

+  18H2O.    (Joly.) 

Sodium  uranyl  arsenate,  Na(U02)As04. 
Ppt.    (Werther,  A.  68.  312.) 


Sodium  zinc  arsenate,  NaZnAsO4. 
Slowly  sol.  in  dil.  acids.    (Lefevre.) 
Na2ZnAs2O7.    As  above.    (Lefevre.) 

Sodium  arsenate  fluoride,  Na3AsO4,  NaF  + 

12H2O. 

Sol.  in  9.5  pts.  H2O  at  25°,  and  2  pts.  at 
75°.  (Briegleb,  A.  97.  95.) 

Sodium  arsenate  stannate,  6Na2O,  2As.>O5, 
SnO2+50H2O. 

More  difficultly  sol.  than  sodium  stannate. 
(Haeffely,  Phil.  Mag.  (4)  10.  290.) 

5Na3AsO4,  Na2SnO3+60H2O.  (Prandtl, 
B.  1907,  40.  2133.) 

Sodium  arsenate  sulphate,  Na8As6Oi9, 

2Na2SO4. 

Sol.  in  H2O.    (Mitscherlich.) 
Na4As2O7,  Na2SO4.    (Setterberg.) 

Sodium  arsenate  tungstate,  Na4As2O7, 

Na2W3O10+20H2O. 
See  Arseniotungstate,  sodium. 

Strontium  arsenate,  Sr3(As04)2. 

Not  attacked  by  boiling  H2O;  easilv  sol.  in 
dil.  acids.  (Lefevre,  A.  ch.  (6)  27.  5.) 

Strontium  pyroarsenate,  Sr2As207. 
Decomp.   by   cold   H2O   into   SrHAsO4-f- 
H2O.    (Lefevre.) 

Strontium    hydrogen    arsenate,    SrHAsO44- 


Insol.  in  cold,  but  decomp.  by  hot  H2O  into 
a  basic,  and  a  sol.  acid  salt.  100  pts.  H2O  at 
15.5°  dissolve  0.284  pt.  (Thompson,  1831.) 

Sol.  in  HC2H3O2,  and  very  easily  in  HC1-+- 

q.    (Kotschoubey,  J.  pr.  49.  182.) 

Sol.  in  HNO3+Aq. 

SrH4(AsO4)2+2H2O.  Partly  sol.  in  H2O. 
Hermann,  Dissert.  1879.) 

Strontium  vanadium   arsenate,  SrHAs04, 

2(V02)H2As04+7^H20. 
See  Arseniovanadate,  strontium. 

Strontium    arsenate    chloride,    3Sr3(AsO4)2, 
SrCl2. 

Insol.  in  H20;  easily  sol.  in  dil.  HNO3+Aq. 
Lechartier,  C.  R.  65.  172.) 

Thallous  arsenate,  Tl3AsO4. 

Sol.  inH2O.    (Willm,  A.  ch.  (4)  5.  5.) 

Thallous  hydrogen  arsenate,  Tl2HAsO4. 
Very  easily  sol.  in  H2O.    (Willm.) 

hallous  dihydrogen  arsenate,  TlH2AsO4. 
Easily  sol.  in  H2O.    (Willm.) 

hallic  arsenate,  TlAsO4-f  2H2O. 

v/wr1^  Sol<  in  HC1+Aq;  decomp. 
y  NH4OH,  or  KOH+Aq.  (Willm.) 


ARSENIMIDE 


69 


Thorium  hydrogen  arsenate,  Th(HAs04)2  + 

6H2O. 

Insol.  in  H2O  or  H3AsO4+Aq.    (Berzelius.) 
Ppt.;  insol.  in  H2O.    (Barbieri,  C.  A.  1911. 

3385.) 
Th(H2As04)4+4H2O.     Decomp.  by  H2O. 

(Barbieri,  I.  c.) 


Tin  (stannous)  arsenate, 

Insol.  in  H2O.    (Lenssen,  A.  114.  113.) 

Tin  (stannic)  arsenate,  2SnO2,  As2O5. 

Ppt.  Insol.  in  H->O  and  dil.  HNO3+Aq. 
(Haeffely,  Phil.  Mag.  (4)  10.  290.) 

Sn3(AsO4)4+6H2O.  Insol.  in  H2O;  sol.  in 
cone.  HCl+Aq,  and  in  aqua  regia;  insol.  in 
HN03+  Aq  or  H2SO4.  (Williams,  Proc.  Soc. 
Manchester,  15.  67.) 

Colloidal..  Very  slowly  sol.  in  H2O,  from 
which  it  is  pptd.  by  HC1,  HNO3,  or  H2SO4+ 
Aq;  also  by  BaCl2,  CaCl2,  NH4C1,  and  FeCl3 
+  Aq,  and  by  AgNO3,  or  KI  +  Aq.  Not  pptd. 
by  alcohol,  HC2H3O2,  HgCL,  Na2CO3,  K2CO3, 
or  (NH4)2CO3+Aq.  The  pptd.  jelly  is  read- 
ily sol.  in  cone,  acids,  and  KOH,  or  NaOH  + 
Aq.  (Williams,  I.e.) 

Tin  (stannous)  arsenate  chloride,  Sn3(AsO4)2, 

SnCl2+2H20. 
Decomp.  on  air.    (Lenssen,  A.  114.  113.) 

Titanium  arsenate  (?). 

Insol.  in  H2O.  Sol.  in  titanic  acid,  arsenic 
acid,  or  HCl+Aq.  Sol.  in  Ti  salts  +Aq. 
(Rose.) 

Titanyl  arsenate,  5TiO2,  2As2O5. 

Sol.  in  acids  without  decomp.  Scarcely 
attacked  by  KOH  or  by  NH4OH+Aq. 
(Reichard,  B.  1894,  27.  1026.) 

Uranous  arsenate,  U3(AsO4)2. 
Ppt. 

Uranous  hydrogen  arsenate,  UH2(AsO4)2  + 
3H2O. 

Ppt.    Sol.  in  HCl+Aq. 
Uranyl  arsenate,  (UO2)HAsO4+4H2O. 

Insol.  in  H2O,  HC2H3Q2,  and  saline  solu- 
tions, as  NH4Cl+Aq;  sol.  in  the  mineral 
acids;  sol.  in  K2CO3+Aq.  (Werther,  A.  68. 
313.) 

(UO2)H4(AsO4)2+3H2O.     (Werther.) 

(UO2)oAs2O7.    Insol.  in  H2O;  sol.  in  acids. 

(UO2)3(AsO4)2  +  12H2O. 

Min.  Trosgerite. 

Vanadium  dihydrogen  arsenate,  (VO2)H2AsO4 
+4H2O. 

Easily  sol.  in  H20.  (Friedheim,  B.  23. 
2600.) 

See  Arseniovanadic  acid. 

Vanadium  zinc  arsenate,  (VO2)2ZnH2(AsO4)2 
2O,  and2(VO2)H2AsO4+6^H2O. 


See  Arseniovanadate,  zinc. 


Vanadyl  arsenate,  (VO)2HAsO4+H2O. 

Very  slowly  sol.  in  H2O;  insol.  in  alcohol; 
easily  sol.  in  HCl+Aq.  (Berzelius.) 

Composition  given  by  Friedheim  (B.  23. 
2600). 

Yttrium  arsenate,  YtHAs04. 

Ppt.  Insol.  in  acetic,  easily  sol.  in  mineral 
acids. 

Zinc  arsenate,  basic,  4ZnO,  As2O5+H2O. 

(Friedel,  J.  B.  1866.  949.) 

Min.  Adamite.  Easily  sol.  in  dil.  HCl+Aq, 
and  is  attacked  by  HC2H3C>2. 

Zinc  arsenate,  Zn3(AsO4)2. 

(deSchulten,  Bull  Soc.  (3)  2.  300.) 

+3H2O.  Ppt.  Sol.  in  HNO3,  and  H3AsO4 
+Aq.  (Kottig,  J.  pr.  48.  182.) 

+8H2O. 

Min.  Kottigile. 

Zinc  arsenate,   acid,  Zn5H2(AsO4)4. 

Easily  sol.  in  cold  HCl+Aq,  less  easily  in 
cold  HNO3.  Sol.  in  KOH,  or  NaOH+Aq 
(Gorguel,  Dissert,  1894.) 

+3H2O.  Insol.  in  H2O;  sol.  in  H3As04,  or 
HNO3+Aq.  (Mitscherlich.) 

+5H2O.  Sol.  in  dil.  HCl+Aq.  (Demel,  B. 
12. 1279.)  Could  not  be  obtained,  (Coloriano, 
Bull.  Soc.  (2)  45.  709.) 

2ZnO,  As2O5.  Very  slowly  decomp.  by 
cold,  rapidly  by  boiling  H2O.  (Lef6vre.) 

ZnHAsO4+H2O.  Insol.  in  H2O.  (Debray, 
Bull.  Soc.  (2)  2.  14.) 

Decomp.  by  hot  H2O  into  4ZnO,  As2O5  + 
H2O.  (Coloriano,  C.  R.  103.  273.) 

Zn(ZnOH)2As2O7+7H2O  (Gorgeul.) 

Zinc  arsenate  ammonia,  Zn3(AsO4)2,  2NH3  + 

3H20. 

Insol.  in  H2O;  sol.  in  acids,  NH4OH,  or 
KOH+Aq.  (Bette,  A.  16.  141.) 

Zirconium  arsenate,  2ZrO2,  As2O5+5/2H2O  = 

(ZrO)HAsO4+MH2O. 
Ppt.    Insol.  in  HoO  or  HCl+Aq.    (Paykull, 
B.  6.  1467.) 

Perarsenic  acid. 
See  Perarsenic  acid. 

Arsenicotungstic  Acid. 

Ammonium  vanadium  arsenicotungstate. 
See  Arsenicovanadicotungstate,  ammonium. 

Arsenicovanadicotungstic  acid. 

Ammonium    arsenicovanadicotungstate, 

16(NH4)oO,   5As2O3,    15V2O3,   26WO3  + 
101H2O. 
SI.  sol.  in  cold,  readily  sol.  in  hot  H2O. 

(Rogers,  J.  Am.  Chem.  Soc.  1903,  26.  308.) 

Arsenimide,  As2(NH)3. 

Decomp.  by  H,,O.  (Hugot,  C.  R.  1904, 
139.  56.) 


70 


ARSENIOARSENIC  ACID 


Arsenioarsenic  acid,  3As2O3,  2As2O5  + 
3H2O. 

Decomp.  by  H2O.    (Joly,  C.  R.  100.  1221.) 

3As2O3,  As2O8+H2O.  Decomp.  by  H2O. 
(Joly.) 

As2O3,  As2O5+H2O.  Decomp.  by  H2O. 
(Joly.) 

See  also  Arsenic  dioxide  pentoxide. 

Arseniochromic  acid. 

Ammonium    arseniochromate,    2(NH4)2O, 
As2O6,  4CrO3+H2O. 

Insol.  in  H2O.  (Friedheim  and  Mozkin, 
Z.  anorg.  1894,  6.  280.) 

3(NH4)2O,  As2O5,  8CrO3.  Decomp.  by 
recryst.  from  H2O.  (Friedheim  and  Mozkin, 
Z.  anorg.  1894,  6.  281.) 

Potassium  arseniochromate,  2K2O,  As2O5, 
4CrO3. 

Decomp.  by  recryst.  from  H2O.  (Friedheim 
and  Mozkin,  Z.  anorg.  1894,  6.  275.) 

2K2O,  As2O6,  4Cr03+H2O.  Decomp.  by 
recryst.  from  H2O.  (Friedheim  and  Moz- 
kin, I.  c.) 

Arseniomolybdic  acid,  As206,  6MoO3  + 
10H2O. 

By  recryst.  from  H2O  the  comp.  with  18H2O 
is  formed.  (Pufahl,  Dissert.  1888.) 

+  16H2O.      Sol.  in  H2O.    (Debray.) 

+  18H2O.  Completely  sol.  in  H2O.  Sp.gr. 
of  sat.  solution  at  18.8°  is  2.21.  Easily  sol.  in 
abs.  alcohol.  Insol.  in  CS2,  liq.  hydrocarbons 
and  CHC13.  (Pufahl,  I.e.) 

As2O5,  7MoO3+14H2O.  (Seyberth,  B.  7. 
391.) 

As2O.6,  18MoO3+28H2O.  Very  sol.  in  H2O. 
Sp.  gr.  of  sat.  solution  at  18.3°  =  2.45  and  1  cc. 
contains  2.16  g.  acid.  Easily  sol.  in  absolute 
alcohol;  insol.  in  CS2,  liquid  hydrocarbons 
and  CHC13.  (Pufahl,  I.e.) 

Sol.  in  ether  with  subsequent  separation 
into  two  layers.  See  Phosphotungstic  acid. 
(Drechsel,  B.  20.  1452.) 

+38H2O.  Efflorescent.  When  recryst. 
comp.  with  28HoO  is  formed.  (Pufahl,  I.e.) 

As2O5,  20MoO3+27H2O.  SI.  sol.  in  HNO3 
+Aq.  (Debray,  C.  R.  78.  1408.) 

Ammonium  arseniomolybdate,  (NH4)2O, 
As2O5,  2MoO3+3H2O. 

(Friedheim,  Z.  anorg.  1894,  6.  28.) 

+4H2O.    (Friedheim,  I.e.) 

(NH4)2O,  As2O5,  6MoO3+2H2O.  SI.  sol. 
in  cold  H2O;  sol.  in  acids.  (Debray.) 

+4H2O.  SI.  sol.  in  cold,  very  easily  sol.  in 
hotH2O.  (Pufahl,  I.e.) 

2(NH4)2O,  As2O5,  6MoO3+6H2O.  SI.  sol. 
in  H2O.  Cannot  be  recryst.  therefrom. 
(Pufahl.) 

+  12H2O.  (Friedheim,  Z.  anorg.  1894,  6. 
31.) 

3(NH4)2O,  As2O5,  6MoO3+4H2O.  (Fried- 
heim, I.e.) 


+8H2O.    (Friedheim,  I.e.) 

(NH4)2O,  2H2O,  7MoO3,  As2O5+4H2O. 
Sol.  in  hot  H2O.  (Seyberth,  B.  7.  391.) 

Not  obtained.    (Pufahl.) 

7fNH4)2O,     2As2O6,     14MoO3+28H2O. 
(Friedheim,  I.e.) 

5(NH4)2O,  As2O6, 16Mo03+5H20.  (Fried- 
heim, Z.  anorg.  1894,  6.  31.) 

5(NH4)2O,  As2O5,  16MoO3+9H2O.  Nearly 
insol.  in  cold,  sol.  in  boiling  H2O.  Easily  sol. 
in  NH4OH+Aq.  (Gibbs,  Am.  Ch.  J.  3.  402.) 

+  12H2O.     (Pufahl,  I.e.) 

2(NH4)20,       As206,        18Mo03+17H20. 

(Pufahl,  I.e.) 

3(NH4)2O,As2O5,18MoO3+14H20.  Very 
sol.  in  H20  and  alcohol.  (Kehrmann,  Z. 
anorg.  1894,  7.  421.) 

3(NH4)2O,  As2O5,  20MoO3.  Easily  sol.  in 
H2O.  (Debray,  C.  R.  78.  1408.) 

3(NH4)2O,  As2O5,  24MoO3+12H2O.  De- 
composed by  H2O,  especially  when  boiling. 
Easily  sol.  in  NH4OH+Aq,  less  easily  sol.  in 
warm  H2SO4  and  boiling  H3AsO4+Aq.  SI. 
sol.  in  molybdic  acid+Aq,  HNO3,  and  cone. 
NH4NO3+Aq.  (Pufahl,  I.e.) 

Barium   arseniomolybdate,   BaO,   As2O5, 
6MoO3  +  10H2O. 

SI.  sol.  in  H2O.  Partially  decomp.  by  boil- 
ing. (Pufahl,  I.e.) 

3BaO,  As2O5,  6MoO3.  SI.  sol.  in  H2O. 
(Pufahl,  I.e.) 

3BaO,  As2O5,  7MoO3.    Ppt.     (Seyberth.) 

3BaO,  As2O5,  18MoO3.  Decomp.  by  H2O. 
(Pufahl,  I.e.} 

Cadmium  arseniomolybdate,  CdO,  2H2O, 
As2O5,  6MoO3+llH2O. 

(Pufahl.) 

3CdO,  3H20,  As206,  18Mo03+33H2O. 
(Pufahl.) 

Caesium  arseniomolybdate,  Cs2O,  As2O5, 
6MoO3. 

SI.  sol.  in  H2O.    (Pufahl,  I.e.) 
4Cs2O,    As2O5,    26MoO3  +  15H2O.      Ppt. 
(Ephraim,  Z.  anorg.  1910,  65.  246.) 

Calcium  arseniomolybdate,  CaO,  As2O5, 
6Mo03  +  10H20. 

Rather  difficultly  sol.  in  cold  H2O.  (Pufahl, 
I.e.) 

3CaO,  As2O5,  6MoO3.  As  Ba  salt.  (Pu- 
fahl, l.c.) 

3CaO,  As2O5,  18MoO3+32H2O.  Very  sol. 
in  H2O.  Solution  sat.  at  18°  has  sp.  gr  = 
2.163.  (Pufahl,  I.e.) 

Cobalt  arseniomolybdate,  CoO,  2H20,  As2O5, 
6MoO3  +  llH2O. 

(Pufahl.) 

3CoO,  3H2O,  As2O5,  18MoO3+33H2O. 
(Pufahl.) 

Cupric  arseniomolybdate,  CuO,  2H2O,  As2O5, 
6MoO3  +  15H2O.  (Pufahl.) 

3CuO,    3H20,    As205,     18MoO3+34H2O. 

(Pufahl.) 


ARSENIOSULPHATE,  POTASSIUM 


71 


Lithium     arseniomolybdate,     Li2O,     As2O5 

6MoO3+14H2O. 
Very  sol.  in  H2O.    (Pufahl,  I.e.) 
3Li2O,  As205,  18MoO3+34H2O.    Solution 

sat.  at  15°  has  sp.  gr.  of  2.481.    (Pufahl,  I.e. 

Magnesium  arseniomolybdate,  MgO,  As2O5 

6Mo03  +  13H20. 
Very  sol.  in  H2O.    (Pufahl,  I.e.) 
3MgO,  As2O5,   18MoO3+36H2O.     Sol.  ir 

H2O.    (Pufahl,  I.e.) 

Manganese  arseniomolybdate,  MnO,  2H20 
As2O5,  6MoO3  +  llH2O. 

(Pufahl.) 

3MnO,  3H2O,  As2O5,  18MoO3+33H20 
(Pufahl.) 

Nickel  arseniomolybdate,  NiO,  2H2O,  As2O5 
6Mo03  +  llH20. 

(Pufahl.) 

3NiO,  3H2O,  As2O5,  18Mo03+34H2O 
(Pufahl.) 

Potassium  arseniomolybdate,  K2O,  As2O6. 
2MoO3+5H2O. 

Sol.  in  H2O.    (Friedheim,  Z.  anorg.  2.  314.) 

K2O,  As2O5,  6MoO3+5H2O.  Sol.  in  hot 
H2O  without  decomp.  (Friedheim,  Z.  anorg 
1892,  2.  330.) 

K2O,  As2O5,  18MoO3+25H2O.  Easily  sol 
in  cold  H2O.  Decomp.  on  dilution.  (Pufahl, 
I.e.) 

3K2O,  As2O5,  18MoO8+26H2O.  Easily 
sol.  in  H2O.  (Pufahl,  I.e.) 

3K20,  As2O5,  20MoO3.  Insol.  in  H2O. 
(Debray,  C.  R.  78.  1408.) 

3K20,  As2O5,  24MoO3+12H20.  Somewhat 
sol.  in  H20  acidified  with  HNO3.  (Pufahl, 
I.e.) 

Rubidium  arseniomolybdate,  3Rb2O,  3As2O5, 
5MoO3+9H2O. 

Easily  sol.  in  H2O.  (Ephraim,  Z.  anorg. 
1910,  65.  241.) 

Rb2O,  As2O5,  6MoO3.  SI.  sol.  in  H20. 
(Pufahl,  I.e.) 

4Rb2O,  As206,  18MoO3+40H2O.  Pptd. 
(Ephraim,  Z.  anorg.  1910,  65.  241-4.) 

Silver  arseniomolybdate,  3Ag2O,   As2O5, 
6MoO3+zH2O. 

(Pufahl,  Leipzig,  1888.) 

6Ag2O,  As2O5,  18MoO3+22H2O.  SI.  sol. 
in  H2O.  Very  sol.  in  NH4OH  and  in  dil. 
HNO8.  (Pufahl,  I.e.) 

7Ag2O,  2As2O5,  36MoO3+30H2O.  SI.  sol. 
in  cold,  easily  sol.  in  hot  H2O  strongly  acidi- 
fied with  HNO3.  (Pufahl,  I.e.) 

Sodium     arseniomolybdate,     Na2O,     As2O5, 

2MoO3+8H2O. 

(Friedheim,  Z.  anorg.  1892,  2.  357.) 
Na2O,  As2O5,  6Mo03+12H2O.     Very  sol. 

in  H20.    Solution  sat.  at  19.8°  has  sp.  gr.  = 

1.678.    (Friedheim,  I.e.) 


3Na2O,  As2O5,  6MoO3+llH2O,  +  12H2O, 
and  +13H20.  SI.  sol.  in  cold  H2O.  (Pufahl, 

3Na2O,  As2O6,  18MoO3+24H20.  Easily 
sol.  in  H2O.  (Pufahl,  I.e.) 

+30H2O.     SI.  sol.  in  cold  H20.    (Pufahl, 

Strontium  arseniomolybdate,  SrO,  As206, 
6Mo03+10H2O.  " 

As  Ba  salt.    (Pufahl,  I.e.) 

3SrO,  As2O6,  6MoO3.  As  Ba  salt.  (Pu- 
fahl, I.e.) 

3SrO,  As2O5,  18MoO3+32H2O.  Very  sol. 
in  H20.  (Pufahl,  l.c.) 

Thallium  arseniomolybdate,  6T12O,  As2O5. 
18Mo03+zH20. 

Ppt.     (Pufahl.) 

3T12O,  3H2O,  As2O5, 18MoO3+3H2O.  Ppt. 
(Pufahl.) 

Zinc  arseniomolybdate,  ZnO,  2H2O,  As206, 
6Mo03+llH20. 

(Pufahl.) 

3ZnO,  As2O5,  18MoO3+37H20.  Very  sol. 
inH2O.  (Pufahl.) 

Arseniophosphovanadicotungstic  acid. 

Ammonium    arseniophosphovanadicotung- 
state,   88(NH4)2O,   2.As2O6,    12P2O6, 
69V2O3,  148WO3+484H2O. 
Sol.  in  H2O.     Insol.  in  alcohol  and  ether. 

(Rogers,  J.  Am.  Chem.  Soc.  1903,  25.  313.) 

Arseniophosphovanadicovanadiotungstic 
acid. 

Ammonium  arseniophosphovanadicovanadio- 
tungstate,  99(NH4)2O,  2As2O5,   12P2O6, 
6V2O3,  66V2O5,  191WO3+522H2O. 
SI.  sol.  in  cold  H2O.    (Rogers,  J.  Am.  Chem. 

Soc.  1903,  25.  314.) 

Arseniophosphovanadiotungstic  acid. 

Ammonium  arseniophosphovanadiotungstate, 
82(NH4)2O,  3As2O6,  12P206,  52V2O6, 
201WO3+567H2O. 

Very  sol.  in  warm  H2O.  Insol.  in  organic 
solvents.  (Rogers,  J.  Am.  Chem.  Soc.  1903, 
25.  312.) 

Arseniosulphuric  acid. 

Ammonium  arseniosulphate,  2(NH4)2O, 

As2O5,  2SO3+3H20. 

Can  be  recryst.  from  H2O.  (Friedheim  and 
VIozkin,  Z.  anorg.  1894,  6.  290.) 

Potassium    arseniosulphate,    2K2O,    As2Ofi, 

2SO3+3H2O. 

(Friedheim  and  Mozkin,  Z.  anorg.  1894,  6 
89.) 

5K2O,  As2O5,  SSO3+6H2O.  (Friedheim 
nd  Mozkin,  Z.  anorg.  1894,  6.  291.) 


72 


ARSENIOSULPHATE,  SODIUM 


Sodium     arseniosulphate,     2Na2O,     As2O6, 

2SO3+3H2O. 

(Friedheim  and  Mozkin,  Z.  anorg.  1894,  6. 
290.) 

Arseniotelluric  acid. 

Ammonium     arseniotellurate,     2(NH4)2O, 
As2O6,  TeO3+4H2O. 

Sol.  in  H2O.  (Weinland,  Z.  anorg.  1901, 
28.  65.) 

4(NH4)2O,  3As2O5,  2TeO3  +  HH2O.  Sol. 
inH2O.  (Weinland.) 

Sodium     arseniotellurate,     2Na2O,     As2O5, 

2TeO3-f9H2O. 
Ppt.    (Weinland,  I.e.) 

Arseniotungstic  acid,  3H2O,  As2O6, 16WO3 
+32H2O  =  H3AsW8O28+16H2O  (o-an- 
hydroarsenioluteotungstic  acid) . 

Sol.  in  H2O.    (Kehrmann,  A.  246.  45.) 

3H2O,  As2O5,  19WO3  (?).  Sp.  gr.  of  sat. 
solution  in  H2O  is  3.279.  (Fremery,  B.  17. 
296.) 

Is  a  mixture  containing  principally 
H8AsW8O28  +  16H2O.    (Kehrmann.) 

As2O6,  18WO3+zH2O.  Sol.  in  H2O. 
(Kehrmann,  Z.  anorg.  1899,  22.  292.) 

Aluminum  ammonium  arseniotungstate. 

See  Aluminicoarseniotungstate,  ammo- 
nium. 

Ammonium    arseniotungstate,    4(NH4)2O, 
2H2O,  As2O5,  6WO3+3H20. 

SI.  sol.  in  cold  H2O  or  HNO3+Aq;  easily 
sol.  in  boiling  H2O.  (Gibbs,  Proc.  Am.  Acad. 
16.  135.) 

7(NH4)20,  AS;06,  14W03,+lftl20.  Very 
si.  sol.  even  in  boiling  H2O.  (Fremery,  I.  c.) 

3(NH4)2O,  As2O5,  16WO3+16H2O  = 
(NH4)3AsWV)28+8H2O.      Sol.  in  H2O. 
(Kehrmann.) 

5(NH4)2O,  As2O6,  17WO3+8H2O.  Can  be 
recryst.  from  H2O  without  decomp.  Decomp. 
by  long  boiling  with  H2O.  (Kehrmann,  Z. 
anorg.  1899,  22.  294.) 

3(NH4)2O,  As2O5,  18WO3  +  14,  or  18H2O. 
Very  sol.  in  cold  H2O.  Can  be  recryst.  from 
H20.  (Kehrmann,  I.e.) 

3(NH4)2O,  As2O5,  21W03+zH2O.  Easily 
sol.  in  H2O.  Easily  decomp.  on  recryst. 
(Kehrmann,  I.e.) 

3(NH4)2O,  As2O5,  24WO3+12H2O.  More 
sol.  in  H2O  than  corresponding  phosphotung- 
state.  (Kehrmann,  I.e.) 

Barium   arseniotungstate,   2BaO,   As2O5, 

16WO3-f-zH2O. 

Sol.  in  H20.    (Pechard,  A.  ch.  (6)  22.  262.) 
7BaO,    As2O6,    22WO3+54H2O.      Sol.    in 
H2O.     Can  be  recryst.  therefrom.     (Kehr- 
mann,   I.e.) 


Potassium  arseniotungstate,  3K2O,  3H2O, 
Aso05,  6WO3. 

Insol.  in  H2O.  Readily  sol.  in  alkali  hy- 
droxides+Aq.  (Gibbs.) 

3K2O,  As2O5, 16WO3  +  16H2O  =  K3AsW8O28 
+8H2O.  Sol.  in  H2O.  (Kehrmann.) 

5K2O,  As2O5,  17WO3+22H2O.  Scarcely 
sol.  in  cold  H2O.  (Kehrmann,  Z.  anorg.  1899, 
22.  295.) 

3K2O,  As2O6, 18WO3  +  14H2O.  Efflorescent. 
(Kehrmann,  I.e.) 

3K2O,  As205,  19WO3  +  16H2O  (?).  Sol.  in 
H20.  (Fremery.) 

Silver  arseniotungstate,  Ag5AsW8O29. 

Insol.  in  H2O  (Kehrmann,  A.  245.  55) ;  per- 
haps identical  with — 

6Ag2O,  As2O5,  16WO3  +  11H2O.  Insol.  in 
H2O.  (Gibbs.) 

Sodium    arseniotungstate,    3Na2O,     As2O6, 

3WO3+20H2O. 
Very  sol.  in  H2O.    (Lefort,  C.  R.  92.  1461.) 

Arsenious  acid,  HAsO2. 

Solubility  of  HAsO2  in  amyl  alcohol +Aq.  at 

25°. 

aw  =mol.  of  HAs02  in  1  1.  of  H2O. 
aa  =mol.  of  HAsO2  in  1  1.  of  amyl  alcohol, 
h  =  partition  coefficient. 


aw 

aa 

h 

0.0449 
0.0446 
0.0887 
0.0892 
0.1800 

0.0082 
0.0083 
0.0164 
0.0161 
0.0324 

5.48 
5.38 
5  41 
5.53 
5.55 

(Auerbach,  Z.  anorg.  1903,  37.  356.) 

Solubility  of  HAs02  in  sat.  H3BO3+Aq  and 
amyl  alcohol. 

aw  =mol.  of  HAsO2  in  1  1.  of  H20. 

aa  =mol.  of  HAsO2  in  1 1.  of  amyl  alcohol. 

h= partition  coefficient. 


aw 

aa 

h 

0.0859 
0.1720 

0.0161 
0.0321 

5.33 
5.35 

(Auerbach,  I.e.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1904,  37.  3601.) 

See  Arsenic  inoxide. 

Arsenites. 

All  arsenites,  except  those  of  the  alkali 
metals,  are  partially  or  wholly  insol.  in  H2O, 
but  easily  sol.  in  acids;  several  are  sol.  in 
(NH4)2S04,  NH4N03,  or  NH4Cl+Aq. 

All  basic  arsenites  are  sol.  in  acids  except 
those  that  give  an  insol.  salt  with  the  bases. 
Many  are  sol.  in  excess  of  As2O3+Aq. 


ARSENITE,  BASIC,  COBALTOUS 


73 


Aluminum  arsenite,  A12O3,  As2O3. 

SI.  sol.  in  boiling  H2O.  Easily  sol.  in  NaOH 
+Aq  and  in  acids.  (Reichard,  B.  1894,  27. 
1029.) 

Aluminum   arsenite   iodide,   Alls,    6As2O3  + 

16H2O. 
(Griihl,  Dissert.  1897.) 

Ammonium  arsenite,  NH4AsO2. 

Very  sol.  in  H2O.    (Luynes,  J.  pr.  72.  180.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014);  (Naumann,  B.  1904,  37.  4328.) 

(NH4)3AsO3  (?).     Sol.  in  HoO.      (Staven- 
hagen,  J.  pr.  1895,  (2)  51.  11.) 
,      (NH4)4As2O5.    Very  sol.  in  H2O.    Insol.  in 
alcohol  or  ether.    (Stein,  A.  74.  218.) 

Could  not  be  obtained.     (Stavenhagen.) 

Ammonium  arsenite  bromide,  2As2O3,  NH4Br. 
SI.  sol.  in  H2O.    (Riidorff,  B.  19.  2679.) 

Ammonium  arsenite  chloride,  As2O3,  NH4C1. 
SI.  sol.  in  H2O.    Sol.  in  warm  dil.  NH4OH 
+Aq.    (Rudorff.) 

Ammonium  arsenite  iodide,  2As2O3,  NH4I. 

SI.  sol.  in  boiling  H2O.  Sol.  in  warm  dil. 
NH4OH+Aq.  (Rudorff.)  . 

Antimony  arsenite  (?). 

Ppt.  Sol.  in  a  small  amount  H2O,  but 
insol.  in  a  large  quantity.  (Berzelius.) 

Completely  sol .  in  KOH  +  Aq.    (Reynolds.) 

Barium  arsenite,  Ba(AsO2)2. 

Easily  sol.  in  H2O  when  recently  pptd.,  but 
insol.  after  being  dried.  Pptd.  from  aqueous 
solution  by  boiling.  (Filhol,  A.  68.  308.) 

Only  si.  sol.  in  H2O.  (Stavenhagen,  J.  pr. 
1895,  (2)  51.  18.) 

Ba3(AsO3)2.  SI.  sol.  in  cold  H2O;  sol.  in 
hot  H2O  and  dil.  acids.  (Stavenhagen,  J.  pr. 
1895,  (2)  51.  17.) 

BaH4(AsO3)2.  Ppt.  (Bloxam,  Chem.  Soc. 
15.  281.) 

+34H2O.  Moderately  sol.  in  cold,  more 
easily  sol.  in  hot  H2O.  Insol.  in  alcohol. 
(Perper,  Dissert.  1894.) 

BaoAs2O5+2H2O.  Easily  sol.  in  H2O. 
(Stavenhagen,  J.  pr.  1895,  (2)  51.  18.) 

+4H2O.  SI.  sol.  in  H2O;  also  somewhat 
sol.  in  alcohol.  (Stein,  A.  74.  218.) 

SI.  sol.  in  H3As04+Aq  and  BaO2H2+Aq. 
(Dumas.) 

Sol.  in  NH4Cl+Aq.  (Wackenroder,  A.  41. 
316.) 

Not  pptd.  from  solutions  containing  Na 
citrate.  (Spiller.) 

B  a  As4O  7 .  Sol .  in  H  2O .  Less  sol .  in  alcohol . 
(Reichard,  B.  1894,  27.  1033.) 

Bismuth  arsenite,  BiAsO3+5H2O  (?). 

Easily  sol.  in  HNO3+Aq.  (Schneider,  J. 
p.  (2)  20.  419.) 


SI.  sol.  in  H2O.  (Stavenhagen,  J.  pr.  1895, 
(2)  51.  35.) 

Cadmium  arsenite,  Cd3(AsO3)2. 

SI.  sol.  in  H2O;  easily  sol.  in  NH4OH+Aq 
and  dil.  acids.  (Stavenhagen,  I.e.) 

Cd2As2O5.  Ppt.  (Reichard,  B.  1898,  31. 
2168.) 

Sol.  in  acids  without  decomp.;  insol.  in 
alkalis.  (Reichard,  B.  1894,  27.  1033.) 

5CdO,  As2O3  +  12H2O.  Not  attacked  by 
KOH,  Ba(OH)2  or  alkali  carbonates +Aq. 
Insol.  in  KCN+Aq.  (Reichard,  Ch.  Z.  1902, 
26.  1145.) 

Caesium  arsenite  bromide,  As2O3,  CsBr. 
Sol.  in  H20.    (Wheeler,  Z.  anorg.  4.  451.) 

Caesium  arsenite  chloride,  As2O3,  CsCl. 
As  above. 

Caesium  arsenite  iodide,  As2O3,  Csl. 
As  above. 

Calcium  arsenite,  Ca(AsO2)2. 

Somewhat  sol.  in  H2O;  sol.  in  Ca(OH)2  + 
Aq  or  As2O3+Aq.  (Simon,  Pogg.  47.  417.) 

Ca3(AsO3)2.    Ppt.    (Kuhn,  J.  B.  1852.  379.) 

Only  si.  sol.  H2O;  readily  sol.  in  dil.  acids. 
(Stavenhagen,  I.e.) 

Sol.  in  H2O,  insol.  in  alcohol.  (Reichard, 
B.  1894,  27.  1036.) 

3CaO,  2As2O3+3H2O.  SI.  sol.  in  H2O; 
easily  sol.  in  NH4Cl+Aq;  sol.  in  As2O3-f  Aq. 
(Stein.) 

CaH4(AsO3)2+o;H2O.  Moderately  sol.  in 
H2O.  Insol.  in  abs.  alcohol.  (Perper,  Dis- 
sert. 1894.) 

Ca2As2O5.  SI.  sol.  in  H2O;  1  pt.  in  3000- 
4000  pts.  H2O.  Alkali  chlorides  increase  sol- 
ubility slightly.  (Stavenhagen,  I.e.) 

SI.  sol.  in  H2O;  insol.  in  H2<D  containing  CaChHz. 
(Berzelius.) 

Not  pptd.  in  presence  of  4000-5000  pts.  HaO.  (Hart- 
ing,  Lassaigne.) 

Not  pptd.  from  solutions  containing  Nth  salts;  and 
when  pptd.  is  sol.  in  (NH^SCh,  NH^NOs,  NH^HsOs, 
and  NHiCl  +Aq.  (Gieseke  and  Schweigger.) 

Sol.  in  NH4AsO2  +Aq.     (Schweigger.) 

Sol.  in  CaCl2+Aq.    (Ordway.) 

Easily  sol.  in  dil.  acids.  Net  pptd.  from  solutions 
containing  sodium  citrate.  (Spiller.) 

Calcium    arsenite    iodide,    CaI2,    3As2O3  + 

12H2O. 

SI.  sol.  in  H2O.  Decomp.  on  heating. 
(Gruhl,  Dissert.  1897.) 

Chromic  arsenite,  CrAsO3. 

Sol.  in  H2O,  but  slowly  decomp.  by  boiling. 
(Neville,  C.  N.  34.  220.) 

Sol.  in  HC1;  repptd.  by  NH4OH+Aq;  sol. 
in  KOH+Aq.  (Reichard,  B.  1894,  27.  1028.) 

Cobaltous  arsenite  basic,  7CoO,  As2O3. 

Very  sol.  in  dil.,  difficultly  sol.  in  cone. 
H2SO4.  Sol.  in  cone.  NaOH  and  in  cone. 
NH4OH+Aq.  (Reichard,  Z.  anal.  1903,  42. 
10.) 


74 


ARSENITE,  COBALTOUS 


Cobaltous  arsenite,  3CoO,As2O3. 

Sol.  KOH+Aq  with  decomp.  (Identical 
with  salt  of  Girard).  (Reichard,  B.  1894,  27. 
1031.) 

+4H2O.  SI.  sol.  in  H2O;  easily  sol.  in 
acids.  (Stavenhagen,  J.  pr.  1895,  (2)  51.  39). 

3CoO,  2As2O3+4H2O.  Sol.  in  HNO3. 
(Girard,  C.  R.  1852,  34.  918.) 

Co3H6(AsO3)4.  Insol.  in  H2O;  sol.  in 
HNO3,  HC1,  or  NH4OH+Aq.  (Proust.) 

Only  sol.  in  KOH,  or  NaOH+Aq  when 
formed  in  a  solution  containing  an  excess  of 
those  reagents.  (Reynoso,  C.  R.  31.  68.) 

Co2As2O5.  Ppt.  (Reichard,  B.  1898,  31. 
2165.) 

Sol.  in  HNO3  and  HCl+Aq.    (Proust.) 

Cupric  arsenite,  Cu(As02)2. 

(Avery,  J.  Am.  Chem.  Soc.  1906,  28.  1161.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

+H2O.  SI.  sol.  in  H2O.  (Stavenhagen, 
I.e.} 

+2H2O.  SI.  sol.  in  H20;  insol.  in  alcohol. 
(Stavenhagen,  I.e.) 

3CuO,  As2O3.    Ppt.    (Stavenhagen,  I.e.) 

2CuO,As2O3.  (Scheele's  green.)  Insol.  in 
H2O;  sol.  in  KOH+Aq,  NH4OH+Aq,  and 
in  most  acids.  Formula  is  Cu3(AsO3)2  + 
2H2O.  (Sharpies,  C.  N.  35.  89.) 

Sol.  in  NH4OH+Aq  without  decomp.  Sol. 
in  KOH+Aq  with  decomp.  (Reichard,  B. 
1894,  27.  1026.) 

Insol.  in  pyridine.  (Schroeder,  Dissert. 
1901.) 

5CuO,  As2O3.  Insol.  in  H2O,  sol.  in  acids, 
NH4OH+Aq  and  cone.  MOH+Aq.  (Reich- 
ard, Ch.  Z.  1902,  26.  1142.) 

zCuO,  2/As2O3.  Min.  Trippk&ite.  Easily 
sol.  in  HNO3  and  in  HCl+Aq. 

Didymium  arsenite,  Di2H3(AsO3)3. 

Ppt.    (Frerichs  and  Smith,  A.  191.  355.) 
Does  not  exist.    (Cleve,  B.  11.  910.) 

Glucinum   arsenite   iodide,    G1I2,    3As2O3  + 

8H20. 
Decomp.  by  H20.    (Gruhl,  Dissert.  1897.) 

Gold  (aurous)  arsenite,  3Au2O,As2O3. 

Decomp.  by  light.  (Reichard.  B.  1894, 
27.  1027.) 

Gold  (auric)  arsenite,  AuAsO3+H2O. 

Very  sol.  in  H2O,  NH4OH+Aq  and  dil. 
acids.  (Stavenhagen,  J.  pr.  1895,  (2)  51.  28.) 

Iron  (ferrous)  arsenite,  FeO,As2O3. 

Decomp.  in  the  air  when  moist;  sol.  in 
NH4OH+Aq  when  freshly  pptd.  (Reichard, 
B.  1894,  27.  1029-30.) 

Fe2As2O5.  Ppt.  Sol.  in  NH4OH+Aq; 
insol.  in  NH4  arsenite,  or  other  NH4  salts + 
Aq.  (Wittstein.) 


Iron  (ferric)  arsenite,  basic,  4Fe2O3,  As2O3  + 
5H2O. 

Ppt.  H2O  extracts  As2O3.  Sol.  in  cone, 
acids  with  separation  of  As2O3.  Acetic  acid 
is  without  action.  (Bunsen  and  Bertholdr 
1834.) 

Sol.  in  KOH,  or  NaOH+Aq. 

Iron  (ferric)  arsenite,  Fe203,As203. 

Sol.  in  NH4OH+Aq  when  freshly  pptd. 
(Reichard,  B.  1894,  27.  1030.) 

Fe4As209.  Ppt.  (Reichard,  B.  1898,  31. 
2170.) 

+7H2O.    Sol.  in  NaOH,  and  KOH+Aq. 

"Ferric  arsenite"  is  si.  sol.  in  A12(SO4)3  + 
Aq.  (Kynaston,  Dingl.  235.  326.) 

Lanthanum  arsenite,  La2H3(AsO3)3. 

Ppt.    (Frerichs  and  Smith,  A.  191.  355.) 
Does  not  exist.    (Cleve,  B.  11.  910.) 

Lead  arsenite,  Pb(AsO2)2+zH2O. 

SI.  sol.  in  H2O.  Insol.  in  KOH,  but  sol.  in 
NaOH+Aq.  (Berzelius.) 

Pb2As2O5.  Insol.  in  H2O,  NH4OH,  NH* 
arsenite,  or  other  NH4  salts +Aq.  (Witt- 
stein.) 

Pb3(As03)2.  Scarcely  sol.  in  H2O;  easily 
sol.  in  HNO3,  .or  HC2H3O2+Aq.  Boiling 
H2O  dissolves  some  As203.  Not  completely 
insol.  in  KOH+Aq.  (Streng,  A.  129.  238.) 

Sol.  in  acetic  acid;  insol.  in  H2O  in  the 
presence  of  ammonium  salts;  sol.  in  NaOH  + 
Aq;  si.  sol.  in  KOH+Aq.  (Reichard,  B. 
1894,  27.  1024.) 

+H2O.  SI.  sol.  in  H2O;  easily  sol.  in  dil. 
acids.  (Stavenhagen,  J.  pr.  1895,  (2)  61.  33. 

Lead  arsenite  chloride,  PbsAs208,  2PbCl2. 

Min.  Ekdemite.  Easily  sol.  in  HNO3+Aq, 
and  warm  HCl+Aq. 

Magnesium  arsenite,  Mg3(As03)2. 

Insol.  in  NH4OH+Aq,  but  sol.  in  a  large 
excess  of  NH4Cl+Aq.  (Rose.) 

Very  sol.  in  boiling  H20  and  in  dil.  acids. 
Sol.  in  NH4Cl+Aq.  (Reichard,  B.  1894,  27. 
1032.) 

Very  sol.  in  H2O  and  dil.  acids.  (Staven- 
hagen, I.e.) 

Mg2As2O6+4H2O.  Hydroscopic.  Very 
sol.  in  H2O  and  acids.  (Stavenhagen,  I.e.) 

3MgO,2As2O3+3H2O,  +  15H2O,   and 
+  18H20.     (Perper,  Dissert.  1894.) 

Magnesium  arsenite  iodide,  MgI2,  3As2O3  + 

12H2O. 

Moderately  sol.  in  H2O.  (Gruhl,  Dissert. 
1897.) 

Manganous  arsenite,  Mn3(AsO3)2+3H2O. 

Sol.  in  H2O;  insol.  in  alcohol;  easily  oxidized 
by  moist  air.  (Stavenhagen,  I.e.) 

3MnO,2As2O3.  (Reichard,  B.  1894,  27. 
1032.) 


ARSENITE,  SILVER 


75 


Mn3H2As4O10+4H2O.  SI.  sol.  in  H2O 
Very  sol.. in  acids  and  alkali.  (Stavenhagen 
Z.c.) 

Mn5As2O8.  Ppt.  (Reichard,  B.  1898,  31 
2165.) 

Mercurous  arsenite,  Hg2O,As2O3. 

Decomp.  by  light.  Decomp.  by  H20 
(Reichard,  B.  1894,  27.  1022.) 

Hg3AsO3.  Only  si.  sol.  in  H2O;  sol.  in 
dil.  acids.  (Stavenhagen,  J.  pr.  1895,  (2)  51 
24.) 

Gradually  and  completely  decomposed 
H2O.    (Reichard,  Ch.  Z.  1902,  26.  1143.) 

Mercuric  arsenite,  Hg3(AsO3)2. 
SI.  sol.  in  H2O.    (Stavenhagen,  I.e.} 
Decomp.  more  easily  by  H2O  than  is  the 

mercurous  comp.     (Reichard,  Ch.  Z.   1902 

26.  1143.) 

2HgO,As2O3.  Not  decomp.  by  boiling 
with  H2O.  Undecomp.  by  boiling  acids 
Decomp.  by  KOH+Aq,  K2CO3+Aq  and 
NH4OH+Aq.  (Reichard,  B.  1894,  27. 1021.) 

Hg5As2O8.  Ppt.  Decomp.  by  boiling  H2O 
Very  si.  sol.  in  H2SO4+HC1.  (Reichard,  B 
1898,  31.  2170.) 

Nickel  arsenite,  Ni3(AsO3)2. 

Insol.  in  H2O;  easily  sol.  in  NH4OH+Aq 
(Proust.) 

Ppt.    (Reichard,  B.  1898,  31.  2165.) 
3NiO,2As2O3.     Sol.  in  NH4OH+Aq  (iden- 
tical with  salt  of  Girard).    (Reichard,  B.  1894, 

27.  1031.) 

+4H2O.  Insol.  in  H2O;  sol.  in  NH4OH  + 
Aq.  .(Proust.) 

Sol.  in  KOH+Aq.  (Girard,  C.  R.  34. 
918.) 

2NiO,  AsoO3.  Insol.  in  H20 ;  sol.  in  NH4OH 
+Aq;  sol.  in  KOH+Aq.  (Reynoso,  C.  R. 
31.  68.) 

Platinum  arsenite,  Pt3(AsO3)4. 

Sol.  in  H2O  and  alcohol;  very  unstable. 
(Stavenhagen,  I.e.) 

Potassium  arsenite,  KAsO2. 

Sol.  in  H2O;  si.  sol.  in  alcohol.  (Pasteur, 
A.  68.  309.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1904,  37.  3601.) 

Does  not  exist.    (Stavenhagen,  I.e.) 

K3AsO3.  Very  sol.  in  H2O;  sol.  in  alcohol. 
(Stavenhagen,  I.e.) 

K4As2O5+6H2O.  Very  sol.  in  H2O;  sol.  in 
alcohol.  (Stavenhagen,  I.e.) 

K2As4O7+2HoO.  Sol.  in  H20;  si.  sol.  in 
alcohol.  (Pasteur,  A.  68.  309.) 

Potassium  arsenite  bromide,  4As2O3,  2KBr. 

More  sol.  in  H2O  than  iodide.  (Schiff  and 
Sestini,  A.  228.  72.) 

2As2O3,  KBr.    (Riidorff,  B.  19.  2675.) 


Potassium  arsenite  chloride,  2As2O3,  KC1. 

Much  more  quickly  sol.  in  hot  H2O  than 
bromide  or  iodide.  (Riidorff,  B.  19.  2675.) 

As2O3,  KC1.    Decomp.  by  H2O. 

Potassium  arsenite  iodide,   3As2O3,   2KI  + 
H2O. 

SI.  sol.  in  cold  H2O;  sol.  in  20  pts.  boiling, 
and  40  pts.  cold  H2O.  (Emmet,  Sill.  Am.  J. 
(2)  18.  583.) 

6KAsO2,  2KI+3H2O.  Sol.  in  H2O  and 
alcohol.  Decomp.  by  acids.  (Harms.) 

2KH(As02)2,  As2O3,  2KI.  SI.  sol.  in  H2O. 
(Harms,  A.  91.  371.) 

2As2O3,  KI.  Very  difficultly  sol.  even  in 
boiling  H20.  Very  easily  sol.  in  KOH+Aq, 
but  much  less  so  in  K2CO3+Aq.  (Rudorff. 
B.  19.  2670.) 

Sol.  in  40  pts.  cold,  20  pts.  hot  H2O;  sol.  in 
alkalies.  (Schiff  and  Sestini,  A.  228.  72.) 

Potassium    arsenite    sulphate,    K3AsO3, 

10K2S04. 
(Stavenhagen,   Zeit.   angew.   ch.    1894,   8. 

Rubidium  arsenite,  RbAsO2. 

Sol.  in  H2O;  aq.  solution  is  alkaline  to 
itmus.  Insol.  in  alcohol.  (Bouchonnet,  C.  R. 
1907,  144.  641.) 

Rubidium  arsenite  bromide,  As2O3,  RbBr. 

Decomp.  by  H2O.  (Wheeler,  Z.  anorg.  4. 
451.) 

Rubidium  arsenite  chloride,  As2O3,  RbCl. 
As  above. 

Rubidium  arsenite  iodide,  As203,  Rbl. 
As  above. 

Silver  arsenite,  AgsAsO3. 

Insol.  in  H-.O.  Not  pptd.  in  presence  of 
20,000  pts.  H2O.  (Harting.) 

1 1.  H2O  dissolves  0.0115  g.  Ag3As03  at  20°. 
Whitby,  Z.  anorg.  1910,  67.  108.) 

Only  si.  sol.  in  H2O  and  in  dil.  acids;  readily 
ol.  in  NH4OH + Aq  and  cone,  acids.  (Staven- 

agen,  I.e.) 

Decomp.  by  light,  by  KOH+Aq  and  by 
STH4OH+Aq.  (Reichard,  B.  1894,  27.  1022- 
3.) 

Easily  sol.  in  HNO3+Aq  and  other  acids. 
Marcet.) 

More  easily  sol.   in   HC2H3O2+Aq  than 

g3PO4;  si.  sol.  in  HC2H3O2+Aq.     (Santos, 

.  N.  38.  94.) 

Insol.  in  KOH+Aq.  (Kuhn,  Arch.  Pharm. 
2)  69.  267.) 

Easily  sol.  in  NH4OH+Aq.    (Marcet.) 

Insol.  in  NH4OH+Aq,  but  sol.  therein  in 
resence  of  alkali  nitrates.  (Santos,  I.e.) 

Incompletely    sol.    in    (NH4)2CO3, 
NH4)2SO4,    or   NH4NO3+Aq.      (Wittstein,. 
lepert.  51.  41.) 


76 


ARSENITE  AMMONIA,  SILVER 


Decomp.  by  NH4Cl+Aq.  Sol.  inKAsO2  + 
Aq.  (Kiihn,  I.e.) 

Not  pptd.  in  solutions  containing  sol. 
citrates.  (Spiller.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,42.3790.)' 

SI.  sol.  in  methyl  acetate.  (Bezold,  Dis- 
sert. 1908.) 

Insol.  in  ethyl  acetate.  (Hamers,  Dissert. 
1906);  (Naumann,  B.  1910,  43.  314.) 

+H2O.  Very  sol.  in  H2O,  NH4OH+Aq 
and  in  dil.  acids.  (Stavenhagen,  J.  pr.  1895, 

(2)  61.  29.) 

2Ag2O,  As2O3.    Ppt.     (Pasteur,  J.  Pharm. 

(3)  13.  395.) 

Could  not  be  obtained.    (Stavenhagen,  I.e.) 
3Ag,O,  2As2O3.     Sol.  in  cold  HC2H3O2  + 

Aq.    (Santos.) 

Sol.  in  NH4OH+Aq  and  in  potassium  ar- 

senite+Aq.    (Girard,  C.  R.  34.  918.) 
Ppt.    (Reichard,  B.  1898,  31.  2167.) 
Could  not  be  obtained.    (Stavenhagen,  I.e.) 

Silver    arsenite    ammonia.    2Ag2O,    As->O3. 

4NH3. 
Insol.  in  H2O  or  alcohol.    (Girard.) 

Sodium  arsenites. 

Correspond  to  potassium  arsenites,  but 
have  not  been  obtained  in  crystalline  form. 
All  are  very  sol.  in  H20.  (Pasteur,  A.  68.  308. 

Na3As03.  Very  sol.  in  H2O.  (Staven- 
hagen, I.e.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1904,  37.  3602.) 

Sodium  arsenite  bromide,  2As2O3,  NaBr. 

Decomp.  by  warm  H2O.  (Riidorff,  B.  21. 
3052.) 

Sodium  arsenite  iodide,  2As2O3,  Nal. 
Decomp.  by  hot  H2O.    (Riidorff.) 

Strontium  arsenite,  Sr3(AsO3)2. 

Sol.  in  H2O.    (Stavenhagen,  I.e.) 

Sol.  in  H2O,  insol.  in  alcohol  (identical  with 
Stein).  (Reichard,  B.  1894,  27.  1036.) 

Sr2As2O5+2H,O.  Quite  easily  sol.  in  H2O. 
(Stein.) 

SI.  sol.  in  H20,  SrO2H2-f  Aq,  or  H3AsO4  + 
Aq.  (Dumas.) 

Very  si.  sol.  in  alcohol.    (Stein.) 

Easily  sol.  in  H2O  and  in  acids.  (Staven- 
hagen, J.  pr.  1895,  (2)  51.  17.) 

Sr3As4O9.  Moderately  sol.  in  H2O.  (Reich- 
ard, B.  1894,  27.  1036.) 

Strontium   arsenite    iodide,    SrI2,    3As2O3  + 

12H2O. 
As  Ba  comp.    (Griihl,  Dissert.  1897.) 

Thallium  arsenite,  Tl3AsG3. 

SI.  sol.  in  H2O  and  alcohol;  easily  sol.  in 
acids,  especially  in  dil.  H2SO4.  (Stavenhager , 
I.e.) 


Tin  (stannous)  arsenite,  Sn3(AsO3)2. 

Ppt.;  decomp.  by  acids  and  alkali.  (Reich- 
ard, B.  1898,  31.  2169.) 

+2H2O.  SI.  sol.  in  H2O.  Easily  sol.  in  dil. 
acids  and  alkalies.  (Stavenhagen,  I.e.) 

Tin  (stannic)  arsenite,  Sn3(AsO3)4+5KH2O. 
SI.  sol.  in  H2O.    (Stavenhagen,  I.e.) 
5SnO2,  2As2O3.    Ppt.    Sol.  in  acids  without 

decomp.    (Reichard,  B.  1894,  27.  1025.) 
Sn7As2On.    Ppt.     (Reichard,  B.  1898,  31. 

2169.) 

Uranium  arsenite,  UO2,  As2O3. 

Insol.  in  NH4OH+Aq;  only  si.  sol.  KOH  + 
Aq.  Sol.  in  acids.  (Reichard,  B.  1894,  27. 
1029.) 

Zinc  arsenite,  ZnO,  As2O3. 

Ppt.  (Avery,  J.  Am.  Chem.  Soc.  1906,  28. 
1163.) 

3ZnO,As2O3.  Sol.  in  acids  without  decomp. 
Easily  sol.  in  NH4OH+Aq.  (Reichard,  B. 
1894,  27.  1033.) 

Arseniovanadic  acid,  As2O5,  V2O5  +2H2O. 

Easily  sol.  in  H20,  but  solution  easily  de- 
composes; crystallizes  from  H2O  with  10H2O. 
Composition  is  vanadium  dihydrogen  arsen- 
ate  (VO2)H2As04.  (Friedheim,  B.  23.  2600.) 

+14,  and  +18H2O.  (Ditte,  C.  R.  102. 
757.)  Could  not  be  obtained.  (Friedheim.) 

3As2O5,  2V2O5.  (Berzelius.)  Correct  for- 
mula is  as  above.  (Friedheim.) 

3H2O,  7As2O5,  6V2O5.  (Gibbs,  Am.  Ch.  J. 
7.  209.)  Could  not  be  obtained.  (Fried- 
heim.) 

3H2O,  5As2O5,  8V2O5+24H20.  (Gibbs.) 
Could  not  be  obtained.  (Friedheim.) 

Ar  s  enio  vanadate  s . 

According  to  Friedheim  (Z.  anorg.  1892, 
2.  319)  the  arseniovanadates  are  double  ar- 
senates  of  VO2  and  NH4. 

Ammonium  arsenio vanadate,   (NH4)20, 
As2O52V2O5,+5H2O. 

Efflorescent  in  dry  air;  si.  sol.  in  cold, 
decomp.  by  hot  H2O.  Composition 
is  ammonium  divanadium  arsenate 
=  (VO2)2(NH4)AsO4+2^H2O.  (Friedheim, 
B.  23.  2600.) 

SI.  sol.  in  cold  H2O.  Somewhat  more  easily 
sol.  in  hot  H2O  with  separation  of  V2O5. 
(Schmitz-Dumont,  Dissert.  1891.) 

2(NH4)2O,  3As2O5  2V2O5,+4H2O.  Can- 
not be  crystallized  from  H2O.  Composition 
is  m  (NH4)2HAs04+2(V02)2H2As04.  (Fried- 
heim.) 

Decomp.  under  H2O  to  (NH4)2O,  2V2O5. 
As2O5+5H2O.  (Schmitz-Dumont,  I.e.) 

5(NH4)2O,  4As2O5,  2V2O5+18H2O.  Sol.  in 
H2O.  (Ditte,  C.  R.  102.  1019.)  Does  not 
exist.  (Friedheim,  B.  23.  2605.) 


ARSENOSOMOLYBDATE,  MANGANESE 


77 


Calcium    arseniovanadate,    2CaO,     3As2O3, 
2V2O5+21H2O  =  CaHAsO4+2(VO2) 
H2AsO4+8H2O. 

Can  be  crystallized  in  presence  of  vanadic 
acid  without  decomp.  (Friedheim.) 

Efflorescent.  Sol.  in  H2O.  (Schmitz- 
Dumont,  I.e.) 

Cobalt  arseniovanadate,  CoO,  As2O5,  V2O5-f 

9H2O  =  Co(VO2)2H2(AsO4)2+8H2O. 
Sol.  in  H2O.    (Friedheim.) 

Copper  arseniovanadate,  CuO,  As2O5,  V2O5+ 

4H2O  =  Cu(V02)2H2(As04)2+3H2O. 
Sol.  in  H2O.    (Friedheim.) 

Magnesium  arseniovanadate,   MgO,  As2O6, 
V205  +  10H20  =  (V02)2MgH2(As04)2  + 
9H2O. 

Sol.  in  H2O.    (Friedheim.) 

Moderately  sol.  in  H2O.  Solution  decomp. 
on  standing.  (Schmitz-Dumont,  I.e.) 

2MgO,  3As2O6  2V2O5,+23H2O  =MgHAsO4 
+2(V02)H2AsO4+9H2O.  Sol.  in  H2O.  (Fried- 
heim.) 

Sol.  in  H20  but  solution  decomp.  on  evap- 
oration. (Schmitz-Dumont,  I.e.) 

Potassium  arseniovanadate,  K20,  As2(>6, 
2V2O5+5H2O  =  (VO2)2KAsO4+2HH2O. 

Sol.  in  H2O.    (Friedheim.) 

SI.  sol.  in  cold  H2O.  Partially  decomp.  on 
heating.  (Schmitz-Dumont.) 

Strontium  arseniovanadate,  2SrO,  3As2O5, 
2V2O5+20H2O  =SrHAsO4+2(V02)2H2 


Sol.  in  H2O.    (Friedheim.) 
+21H2O.    Easily  sol.  in  H2O.     (Schmitz- 
Dumont.) 

Zinc  arseniovanadate,  ZnO.  As2O5,  V2O6 


Sol.  in  H2O.    (Friedheim.) 

2ZnO,  3As2O5,  2V2O6+5H2O,  and+18H20 
=  ZnHAsO4+2(VO2)2H2AsO4,  and+6^H20. 
Sol.  in  H2O.  (Friedheim.) 

Arseniovanadicotungstic  acid. 

Ammonium  arsenic  vanadicotungstate, 
17(NH4)2O,2As2O6,14i^V2O3,20WO8+ 
98H2O. 

SI.  sol.  in  cold  H2O.  Readily  sol.  in  boiling 
H2O.  Insol.  in  alcohol,  ether,  benzene,  CS2, 
CHC13,  acetone,  nitrobenzene,  aniline  and 
acetic  anhydride.  (Rogers,  J.  Am.  Chem. 
Soc.  1903,  25.  307.) 

Arseniovanadicovanadic  acid. 

Ammonium  arseniovanadicovanadate, 

5(NH4)2O,    12As2O6,    12V02,    6V2O5+ 
7H20. 

SI.  sol.  in  cold,  sol.  in  hot  H2O,  from  which 
crystallizes  — 

4(NH4)2O,  9As2O5,  9VO2,  8V2O5+HH2O. 
Sol.  in  H2O.  (Gibbs,  Am.  Ch.  J.  7.  209.) 


Arseniovanadicovanadiotungstic  acid. 


Ammonium  arsenic vanadicovanadiotungstate , 
+73H20. 


17(NH4)2O,2As2O6,7V2O5,4V2O3,32l 


SI.  sol.  in  cold,  readily  sol.  in  boiling  H20. 
(Rogers,  J.  Am.  Chem.  Soc.  1903,  25.  310.) 

Arseniovanadiotungstic  acid. 

Ammonium  arseniovanadiotungstate, 

18(NH4)2O,  2As206,    13V2O6,   39WO3  + 
88H2O. 

Sol.  in  H2O.  Insol.  in  organic  solvents. 
(Rogers,  J.  Am.  Chem.  Soc.  1903,  25.  306.) 

Arseniuretted  hydrogen,  AsH3. 
See  Arsenic  hydride. 

Arsenochromic  acid. 

Potassium  arsenochromate,  K4Cr2As2Oi6+ 
12H20. 

Sol.  in  moderately  cone,  mineral  acids. 
(Tarugi,  C.  C.  1897,  II.  724.) 

K7Cr3As5O22+24H2O.  Ppt.  Sol.  in  dil. 
warm  acids.  (Tarugi.) 

Potassium  hydrogen  arsenochromate, 

K4H6Cr3As2O16. 
(Tarugi,  C.  C.  1897,  II.  724.) 

Arsenosoarseniotungstic  acid. 

Potassium  arsenosoarseniotungstate,  10K2O, 

4As2O5,  As2O3,  21WO3+26H2O.   - 
Precipitate.    Sol.  in  a  large  amount  of  hot 
H2O.    (Gibbs,  Am.  Ch.J.  7.313.) 

Arsenosomolybdic  acid. 

Ammonium   arsenosomolybdate,   3(NH4)2O, 

5As203,  12MoO3+24H2O. 
SI.  sol.  in  H2O.    (Gibbs,  Am.  Ch.  J.  7.  313.) 

Ammonium  barium  arsenosomolybdate, 

3(NH4)2O,    2BaO,    5As2O3,    10MoOs  + 
50H2O. 
Ppt.    (Ephraim,  Z.  anorg.  1910,  66.  57.) 

Ammonium  cupric  arsenosomolybdate, 

(NH4)2O,  CuO,  2As2O3,  4MoO3+2H2O, 
and  2(NH4)20,  CuO,  3As203,  6MoO3  + 
13H2O. 
Ppts.    (Ephraim,  Z.  anorg.  1910,  66.  58.) 

Barium  arsenosomolybdate,  3BaO,  2As2O8, 

8Mo03  +  13H2O. 
Very  si.  sol.  in  H2O.    (Gibbs.) 

Copper  arsenosomolybdate,  2CuO,   3As2O3, 

6MoO3. 

Sol.  inH2O.    (Gibbs.) 
Manganese      arsenosomolybdate, 


3As2O3,     6MoO3+6H2O, 
Insol.  in  H2O.     (Gibbs.) 


2MnO, 
2O. 


78 


ARSENOSOMOLYBDATE,  POTASSIUM 


Potassium  arsenosomolybdate,  3K2O,  As2O3, 
5MoO3+3H2O. 

Easily  sol.  in  H2O.  (Ephraim,  Z.  anorg. 
1910,  66.  54.) 

3K2O,  As2O3,  8MoO3  +  18H2O.  Easily  sol. 
in  H20.  (Ephraim.) 

Sodium  arsenosomolybdate,  Na2O,  As2O3, 
2MoO3+6H2O.  ' 

Easily  sol.  in  H2O.  (Ephraim,  Z.  anorg. 
1910,  66.  56.) 

2Na2O,  As203,  4MoO3+13H2O.  Ppt. 
(Ephraim.) 

Zinc  arsenosomolybdate,  2ZnO,  3As2O3, 

6MoO3+6H2O. 
Sol.inH20.    (Gibbs.) 

Arsenosophosphotungstic  acid. 

Potassium  arsenosophosphotungstate,  10K2O, 
14As2O3,  3P2O6,  32WO3+28H2O. 

Moderately  sol.  in  cold,  very  easily  in  hot 
H2O.  (Gibbs.) 

7K2O,  2As2O3,  4P205,  60WO3+55H2O. 
Sol.  in  hot  H2O  with  decomp.  (Gibbs.) 

Potassium  sodium  arsenosophosphotungstate, 
5K2O,  Na2O,  2As2O3,  2P2O5,  12WO3  + 
15H2O. 
(Gibbs,  Am.  Oh.  J.  7.  313.) 

.  Arsenosotungstic  acid. 

Ammonium    arsenosotungstate,    7(NH4)2O, 
18W03+18H2O. 


Sol.  inH2O.     (Gibbs.) 

Barium    arsenosotungstate,    4BaO,    As2O3, 

9W03+21H20. 
Precipitate.   'Nearly  insol.  in  H2O.  (Gibbs.) 

Sodium  arsenosotungstate,  9Na2O,  8As2O3, 

16WO3+55H2O. 

Very  sol.  in  H2O.    (Gibbs,  Am.  Ch.  J.  7. 
313.) 

Arsenyl  bromide,  AsOBr. 

H2O  dissolves  out  As2O3:  insol.  in  alcohol. 
(Serullas.) 

+H2O.    (Wallace,  Phil.  Mag.  (4)  17.  122.) 
As8O9Br6  =  2AsBr3,  3As2O3  +12H2O. 

Arsenyl  bromide  with  MBr. 
See  Arsenite  bromide,  M. 

Arsenyl  chloride,  AsOCl. 
Sol.  in  H2O  with  decomp. 
+H2O.    (Wallace,  Phil.  Mag.  (4)  16.  358.) 
As3O4Cl.    (WaUace.) 

Arsenyl  chloride  with  MCI. 
See  Arsenite  chloride,  M. 
Arsenyl   potassium  fluoride,  AsOF3,   KF  + 

(Marignac,  A.  146.  237.) 


Arsenyl  iodide,  As8I2On  =  2AsOI,  3As2O3  + 
12H20. 

Decomp.  by  H2O.  (Wallace,  Phil.  Mag.  (4) 
17.  122.) 

SI.  sol.  in  cold  H2O,  less  sol.  in  alcohol. 
(Plisson,  J.  Pharm.  14.  46.) 

Arsenyl  iodide  with  MI. 
See  Arsenite  iodide,  M. 

Arsenyl  sulphoiodide,  AsiJgSeOa. 

Scarcely  attacked  by  cold  H2O.  Boiling 
H2O  extracts  AsI3.  Decomp.  by  hot  HNO3  or 
H2SO4.  Easily  sol.  in  KOH,  or  NH4OH  +  Aq. 
(Schneider,  J.  pr.  (2)  36.  513.) 

Arsine. 
See  Arsenic  hydride. 

Atmospheric  air. 
See  Air,  atmospheric. 

Auriamine,  Au(OH)2NH2. 

(Jacobsen,  C.  R.  1908,  146.  1214.) 
Zhauriamine,  Au2(OH)4NH. 

(Jacobsen,  C.  R.  1908,  146.  1214.) 

O^£0?/2'£L111*1£III11I1G«  .N-A-Us.  JNiis. 

Decomp.  by  H2O  into  NAu3.  (Raschig,  A. 
235.  341.) 

Auric  acid,  HAu2O4. 

Sol.  in  HBr,  or  HCl+Aq.  (Kruss,  B.  19. 
2546.) 

Ammonium  aurate. 

See  Auroamidoimide. 
Barium  aurate,  BaAu204+5H2O. 

SI.  sol.  in  H2O.  (Weigand,  Zeit.  angew.  Ch. 
1905,  19.  139.) 

+6H2O.  Sl.sol.inH2O.  Sol.  in  dil.  H2SO4 
and  in  dil.  HNO3.  Sol.  in  HC1.  Decomp.  by 
alcohol.  (Meyer,  C.  R.  1907,  145.  806.) 

Calcium  aurate  (?). 

Insol.  in  H2O;  sol.  in  CaCl2+Aq.  (Fremy, 
A.  ch.  (3)  31.  485.) 

CaAu204+6H20.  As  Ba  salt.  (Meyer, 
C.  R.  1907,  145.  806.) 

Magnesium  aurate  (?). 

Ppt.  Insol.  in  H2O;  sol.  in  MgCl2+Aq. 
(Pelletier.) 

Potassium  aurate,  KAuO2+3H20. 

Very  sol.  in  H2O,  and  easily  decomp. 
(Fremy,  A.  ch.  (3)  31.  483.) 

Sol.  in  alcohol;  the  solution  in  alcohol  does 
not  decomp.  below  50°.  (Figuier,  A.  ch.  (3) 
11.  364.)  . 

Potassium  aurate  sulphite,  KAuO2,  2K2SO3  + 
5H2O. 

Sol.  in  H2O  with  decomp.  Nearly  insol. 
in  alkaline  solutions.  (Fremy,  A.  ch.  (3)  31. 

485.) 


BARIUM  AMMONIA 


79 


Sodium  aurate,  Na2Au2O4+2H2O. 

Sol.  in  H2O.  Sol.  in  dil.  H2SO4,  dil.  HNO3, 
and  HC1  with  decomp.  Decomp.  by  alcohol. 
(Meyer,  C.  R.  1907,  146.  806.) 

Strontium  aurate,  SrAu2O4+6H2O. 

As  Ba  salt.    (Meyer.) 

Auriimide  chloride,  Au(NH)Cl. 
(Raschig.) 

Auriimide   nitrate,   Au2N2H2O,   2HNO3,    or 
AuN,    HNO3+}^H2O,    or   Au2O(NH)2, 
2HN03. 
Not  deliquescent.     Decomp.  by  hot  H2O 

into  Au2O(NH)2.    (Schottlander,  J.  B.  1884. 

453.) 

Auroamidoimide,  Au(HN)NH2+3H2O. 

(Fulminating  gold.)  Insol.  in  H2O;  not 
attacked  by  dil.  acids;  sol.  in  cone,  acids, 
and  in  moderately  dil.  acids,  when  freshly  pre- 
cipitated. Insol.  in  alkalies  or  alcohol.  Sol. 
inKCN+Aq. 

Tnauroamine,  Au3N+5H2O. 

Not  decomp.  by  boiling  dil.  acetic  acid, 
HNO3,  or  H2SO4.  (Raschig,  A.  1886,  235. 
349.) 

Auricyanhydric  acid,  HAu(CN)4 +1^H2O. 
Easily  sol.  in  H2O,  alcohol,  or  ether. 
See  also  Bromauricyanides. 

Chlorauricyanides. 

lodauricyanides. 

Ammonium  auricyani'de,  NH4Au(CN)4. 

Easily  sol.  in  H2O  or  alcohol.  Insol.  in 
ether. 

Cobaltous  auricyanide,  Co[Au(GN)4]2+9H2O. 
SI.  sol.  in  cold,  easily  in  hot  H2O.    SI.  sol. 
in  alcohol.    (Lindbom.) 

Potassium  auricyanide,  KAu(CN)4+l^H20. 
Efflorescent.    SI.  sol.  in  cold,  easily  in  hot 
H2O.    Easily  sol.  in  alcohol. 

Silver  auricyanide,  AgAuCN4. 

Insol.  in  H2O  or  HNO3+Aq.  Sol.  in 
NH4OH+Aq. 

DiGLUTodiaxnine  nitrate. 
See  Auriimide  nitrate. 

Aurobromhydric  acid. 
See  Bromauric  acid. 

Aurobromic  acid. 

See  Bromauric  acid. 

Aurochlorhydric  acid. 
See  Chlorauric  acid. 

Aurochloric  acid. 
See  Chlorauric  acid. 


Aurocyanhydric  acid. 
Aurocyanides  with  MCN. 
See  Cyanide,  aurous  with  MCN. 

Azinosulphonic  acid. 
Ammonium  azinosulphonate,  N3SO3NH4. 
(Traube,  B.  1914,  47.  944.) 
Barium  azinosulphonate,  (N3SO3)2Ba. 
(Traube,  B.  1914,  47.  944.) 

Potassium  azinosulphonate,  N3SO3K. 

Easily  sol.  in  H20.  Can  be  cryst.  from 
boiling  abs.  alcohol,  (Traube,  B.  '1914,  47. 
943.) 

Sodium  azinosulphonate,  N3SO3Na. 
(Traube,  B.  1914,  47.  944.) 

Azoimide,  HN3. 

Miscible  with  H2O  and  alcohol.  (Curtius 
and  Radershausen,  J.  pr.  (2)  43.  207.) 

Stable  in  aq.  solution ;  decomp.  slowly  by  dil. 
boiling  HC1.  (Curtius,  J.  pr.  1898,  (2)  58. 
265.) 

For  salts  of  HN3,  see  azoimide  of  metal 
under  metal. 

Azoimide,  hydroxylamine,  N3H,2NH2OH. 

Sol.  in  H20.  Gradually  volatilizes  at  ord. 
temp.  (Dennis,  J.  Am.  Chem.  Soc.  1907,  29. 

22.) 

Azophosphoric  acid. 
See  Pf/rophosphamic  acid. 

Dewtezophosphoric  acid. 

See  Pyropb.osphodia.ndc  acid. 

Barium,  Ba. 

Decomp.  by  H2O  and  abs.  alcohol.  (Guntz, 
C.  R.  1901,  133.  874.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  827.) 

Barium  amalgam,  BaHg13. 

Stable  in  contact  with  liquid  amalgam  up 
to  30°.  Can  be  cryst.  from  Hg  without  de- 
comp. if  temp,  does  not  exceed  30°.  (Kerp, 
Z.  anorg.  1900,  25.  68.) 

BaHg12.  Stable  in  contact  with  liquid 
amalgam  from  30°- 100°.  Can  be  cryst.  from 
Hg  without  decomp.  at  any  temp,  within 
these  limits.  (Kerp.) 

Barium  amide,  Ba(NH2)2. 

B.-pt.  280°.    (Mentrel,  C.  C.  1903, 1.  276.) 
Decomp.  by  H2O.     (Guntz  and  Mentrel, 

Bull.  Soc.  1903,  (3)  29.  578.) 

Barium  potassium  amide. 

See  Potassium  ammonobarate. 
Barium  ammonia,  Ba(NH3)6. 

Takes  fire  in  the  air.  Only  si.  sol.  in  liquid 
NH3.  Violently  decomp.  by  H2O.  (Mentrel, 
C.  R.  1902,  135.  740.) 


80 


BARIUM  ARSENIDE 


Barium  arsenide,  Ba3As2. 

Decomp.  by  H2O.  (Lebeau,  C.  R.  1899 
129.  48.) 

Barium  azoimide,  Ba(N3)2. 

Very  si.  hydroscopic;  explosive. 
12.5  pts.  are  sol.  in  100  pts.  H2O  at  0° 

16.2  "     "      "     "  100  "     H2O   "10.5 
16.7    "     "      "     "  100  "     H2O   "  15° 

17.3  "     "      "    "  100  "     H2O   "  17° 
0.0172  pts.  are  sol.  in  100  pts.  abs.  alcohol  at 
16°. 

Insol.  in  ether.     (Curtius,  J.  pr.  1898,  (2. 
58.  290.) 
See  also  Barium  nitride. 

Barium  boride,  BaB6 

Sol.  in  fused  oxidizing  agents,  not  decomp 
by  H2O;  insol.  in  aq.  acids;  si.  sol.  in  cone 
H2SC>4,  sol.  in  dil.  and  cone.  HNO3.  (Moissan 
C.  R.  1897,  125,  634.) 

Barium  sw&bromide  sodium  bromide,  BaBr, 

NaBr. 

Decomp.  by  H2O.  (Guntz,  C.  R.  1903, 
136.  750.) 

Barium  bromide,  BaBr2,  and  +2H2O. 

100  pts.  H2O  dissolve— 
at  0°     20°    40°    60°     80°    100° 

98     104     114     123     135     149  pts.  BaBr2. 

Sat.  BaBr2+Aq  contains  at: 
—20°  —9°    +7°     16°      19°     40° 
45.7     46.5   48.5    48.8    49.3    50.9%BaBr2 
71°    76°    77°   104°  145°  160°  175° 
55.1  55.555.656.6  60.5  59.4  60.3%BaBr2 
(Etard,  A.  ch.  1894,  (7)  2.  540.) 
Sp.  gr.  of  BaBr2+Aq  at  19.5°  containing: 
5          10        15        20        25        30%BaBr2 
1.045  1.092  1.114  1.201  1.262  1.329 


35 
1.405 


40 
1.485 


45 
1.580 


50      55%BaBr2. 
1.685     1.800 


(Kremers,  Pogg.  99.  444,  calculated  by 
Gerlach,  Z.  anal.  8.  285.) 

BaBr2+Aq  containing  7.74%  BaBr2  has 
•sp.gr.  20°/20°=  1.0716. 

BaBr2+Aq  containing  16.76%  BaBr2  has 
sp.  gr.  20°/20°  =  1.1674. 

(Le  Blanc  and  Rohland.  Z.  phys.  Ch.  1896, 
19.  279.) 

Sat.  BaBr2+Aq  boils  at  113°.     (Kremers, 
Pogg.  99.  43.) 

Solubility  in  BaI2+Aq  at  t°. 


t° 

Sat.  solution  contains 

%    BaBr2 

%  BaI2 

—16 
—-16 
+60 
135 
135 
170 
210 

4.7 
5.0 
5.5 
9.3 
9.0 
11.0 
14.9 

57.9 
59.0 
66.0 
67.3 
67.2 
67.4 
67.7 

(Etard,  A.  ch.  1894,  (7)  3.  287.) 

Very  sol.  in  absolute  alcohol.    (Hiinefeld.) 

100  pts.  absolute  methyl  alcohol  dissolve  50 
pts.  BaBr2  at  22.5°. 

100  pts.  absolute  ethyl  alcohol  dissolve  3 
pts.  BaBr2  at  22.5°.  (de  Bruyn,  Z.  phys.  Ch. 
10.  783.) 

Sat.  solution  in  87%  alcohol  contains  6% 
BaBr2.  (Richards,  Z.  anorg.  3.  455.) 

100  pts.  absolute  methyl  alcohol  dissolve 
45.8  pts.  BaBr2+2H2O  at  15°. 

100  pts.  93.5%  methyl  alcohol  dissolve 
27.3  pts.  BaBr2+2H2O  at  15°. 

100  pts.  50%  methyl  alcohol  dissolve  4  pts. 
BaBr2+2H2O  at  15°.  (de  Bruyn,  Z.  phys. 
Ch.  10.  787.) 

100  g.  BaBr2+CH3OH  contain  0.4  g.  BaBr2 
at  the  critical  temp.  (Centnerszwer,  Z.  phys. 
Ch.  1910,  72.  437.) 

At  15°,  1  pt.  by  weight  is  sol.  in: 
36  pts.  methyl  alcohol,  sp.  gr.  0.709 
207    "    ethyl          "          "     "   0.8035 
652    "    propyl        "         "     "   0.8085 

(Rohland,  Z.  anorg.  1897,  15.  413.) 

Nearly  insol.  in  boiling  amyl  alcohol,  10 
ccm.  dissolving  only  an  amt.  equal  to  1.3  mg 
BaO.  (Browning,  Sill.  Am.  J.  144.  459.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328;  Eidmann,  C.  C.  1899,  II.  1014.) 

Insol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1370.) 

Difficultly  sol.  in  methyl  acetate.  (Nau- 
mann, B.  1909,  42.  3789.) 

Insol.  in  ethyl  acetate.  (Naumann,  B.  1910, 
43.  314.) 

Barium  cadmium  bromide,  BaBr^  CdBr2-f- 
Sol.  in  H20.    (v.  Hauer,  W.  A.  B.  20.  40.) 

Barium  rhodium  bromide. 
See  Bromorhodite,  barium. 

Barium  bromide  ammonia,  BaBr2,8NH3. 

Decomp.  by  H2O.  (Joannis,  C.  R.  1905. 
140.  1244.) 

Barium  bromide  hydrazine,  BaBr2,  2N2H4. 

Hydroscopic.  Very  sol.  in  H2O.  Insol.  in 
alcohol.  (Franzen,  Z.  anorg.  1908,  60.  291.) 

Barium  bromofluoride,  BaBr2,BaF2. 

Insol.  in  and  undecomp.  by  boiling  alcohol. 
Sol.  in  HBr  and  in  HNO3.  Decomp.  by  H2O, 
hot  H,S04,  dil.  HC1,  dil.  HN03,  or  dil.  acetic 
icid.  (Defacqz,  C.  R.  1904,  138.  199.) 

Barium  carbide,  BaC2. 

Decomp.  by  H2O.  (Maquenne,  C.  R.  144. 
60.) 

Sp.  gr.  3.75.  Easily  decomp.  by  H2O  and 
dil.  acids.  (Moissan,  Bull.  Soc.  1894,  (3)  11. 
008.) 


BARIUM  CHLORIDE 


81 


Barium  carbonyl,  Ba(CO)2. 
Sol.  in  H2O.     (Guntz  and  Mentrel,  Bull. 
Soc.  1903,  (3)  29.  586.) 

Barium  sw&chloride,  BaCl. 
Decomp.  by  H2O.     (Guntz,  C.  R.  1903, 
136.  751.) 

Barium  sw&chloride  sodium  chloride,  BaCl, 
NaCl. 
Decomp.  by  H2O.     (Guntz,  C.  R.  1903, 
136.  750.) 

Barium  chloride,  BaCl2,  and  +2H2O. 
Permanent  in  dry  air. 

100  pts.  H2O  at  t°  dissolve  (a)  pts.  BaCh  and  (6) 
pts.  BaCh+2H2O. 

Solubility  in  100  pts.  H2O  at  t°. 

t° 

Pts. 
BaCh 

t° 

Pts. 
BaCh 

t° 

Pts. 
BaCh 

0 
1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
34 
35 

30.9 
31.2 
31.5 
31.7 
31.9 
32.2 
32.4 
32.6 
32.8 
33.1 
33.3 
33.5 
33.8 
34.0 
34.2 
34.5 
34.7 
35.0 
35.2 
35.5 
35.7 
36.0 
36.2 
36.5 
36.7 
37.0 
37.2 
37.5 
37.7 
38.0 
38.2 
38.5 
38.7 
39.0 
39.2 
39.5 

36 
37 
38 
39 
40 
41 
42 
43 
44 
45 
46 
47 
48 
49 
•50 
51 
52 
53 
54 
55 
56 
57 
58 
59 
60 
61 
62 
63 
64 
65 
66 
67 
68 
69 
70 

39.7 
40.0 
40.2 
40.5 
40.7 
41.0 
41.3 
41.6 
41.9 
42.2 
42.5 
42.7 
43.0 
43.3 
43.6 
43.9 
44.2 
44.4 
44.7 
45.0 
45.3 
45.6 
45.9 
46.2 
46.4 
46.7 
47.0 
47.3 
47.6 
47.9 
48.2 
48.5 
48.8 
49.1 
49.4 

71 
72 
73 

74 
75 
76 
77 
78 
79 
80 
81 
82 
83 
84 
85 
86 
87 
88 
89 
90 
91 
92 
93 
94 
95 
96 
97 
98 
99 
100 
101 
102 
103 
104 
104.1 

49.7 

50.0 
50.3 
50.6 
50.9 
51.2 
51.5 
51.8 
52.1 
52.4 
52.7 
53.0 
53.3 
53.6 
54.0 
54.3 
54.6 
55.0 
55.3 
55.6 
55.9 
•56.2 
56.6 
56.9 
57.2 
57.6 
57.9 
58.2 
58.5 
58.8 
59.2 
59.5 
59.8 
60.2 
60.3 

t° 

a 

b 

t°               a              b 

15.64 
49.31 

34.86 
43.84 

43.50 
55.63 

74.89      59.94      65.51 
105.48      59.58      77.89. 

(Gay-Lussac,  A.  ch.  (2)  11.  309.) 

100  pts.  H2O  at  t°  dissolve  32.62  +0.271U  pts.  BaCh. 
(Kopp.) 

100  pts.  H2O  dissolve  pts.  BaCh  +2H2O  at  t°. 

t° 

Pts. 
BaCl»+2HiO 

,o                    Pts. 
BaCh+2H20 

16.25 
20.00 
22.50 
37.50 
50.00 

39 
42 
43 
51 
65 

.66 
.22 
.7 
.0 
.0 

62.50               48.0 
75.00               63.0 
87.00               65.0 
100                     72.0 

(Brandes.) 

Sol.  in  2.67  pts.  H2O  at  18.75°.    (Abl.) 
1  pt.  BaCh  is  sol.  in  2.86  pts.  H2O  at  15.5°,  and  1.67 
pts.  at  boiling  temp.     (M.  R.  and  P.) 
100  pts.  H2O  at  15.5°  dissolve  20  pts.  BaCh,  and  43 
pts.  at  87.7°.     (Ure's  Diet.) 

Solubility  in  100  pts.  H2O  at  t°. 

(Mulder,  calculated  from  his  own  and  other 
observations.    Scheik.    Verhandel.  1864.  45.) 

The  saturated  solution  contains  — 
60.3  pts.  BaCl2  to  100  pts.  H2O,  and  boils  at 
104.1°.    (Mulder.) 
60.1  pts.  BaCl2  to  100  pts.  H20,  and  boils  at 
104.4°.    (Legrand.) 
61.8  pts.  BaCl2  to  100  pts.  H2O,  and  boils 
at  104.5°.    (Griffith.) 
59.58  pts.  BaCl2  to  100  pts.  H2O,  and  boila 
at  105.48°  (Gay-Lussac);  at  106°  (Kremers). 
54.1  pts.  BaCl2  to  100  pts.  H20,  and  forms 
crust  at  104.4°;  highest  temperature  observed, 
104.9°.    (Gerlach,  Z.  anal.  26.  426.) 

Sat.  BaCl2-f-Aq  contains  at: 

t 

Pts. 
BaCh 

,0                           PtS. 

i                   BaCh 

0 
12.2 
38.4 
62^75 

31.1 
33.9 
41.2 
47.7 

77.5                 51.9 
95.65                57.7 
102.5                 58.9 
105                     59.7 

(Nordenskiold,  Pogg.  136.  316.) 
100  pts.  H2O  dissolve  pts.  BaCh  at  t°. 

t° 

Pts. 
BaCh 

,0                    Pts. 
BaCh 

9 
30 
37 

33.2 
38.1 
40.0 

50                   43.7 
58                   45.9 

(Gerardin,  A.  ch.  (4)  5.  143.) 

1  pt.  BaCl2+2H2O  is  sol.  in  2.18  pts.  H20 
at  21.5°,  and  the  solution  has  sp.  gr.  =  1.2878. 
(Schiff,  A.  109.  326.) 

1  pt.  anhydrous  BaClo  is  sol.  in  2.86  pts. 
H2O  at  15°.  (Gerlach.) 


100°    130°     144°     160°     180°    215° 
36     37.3    37.5    38.9    40.7    43.1%BaCl2 
(fitard,  A.  ch.  1894,  (7)  2.  535.) 

Aq.  solution  contains  27.6%  BaCl2  at  30°. 
(Shreinemakers,  C.  C.  1910, 1.  9.) 


82 


BABIUM  CHLORIDE 


Solubility  of  BaCl2+2H2O  in  H2O  equals 
1.745  mol.-litre  at  30°.    (Masson,  Chem.  Soc. 
1911,  99.  1136.) 

BaCh+Aq  sat.  at  8°  has  sp.  gr.  1.27.     (Anthon.) 
BaCh+Aq  sat.  at  15°  has  sp.  gr.  1.282.    (Michel  and 
Krafft.) 
BaCh+Aq  sat.  at  18.1°  has  sp.  gr.  1.285,  and  con- 
tains 44.31  pts.  BaCh+2H2O  to  100  pts.  H2O.     (Kar- 
sten.) 

Sp.  gr.  of  BaCh+Aq  at  19.5°. 

Sp.  gr. 

of  BaCl2+Aqat20°. 

g.  mols.  BaCh  per  1. 

Sp.  gr. 

0.01 

0.025 
0.05 
0.075 
0.10 
0.25 
0.40 

1 
1 

1 
1 
1 
1 

1 

.001878 
.00475 
.00929 
.01369 
.  01766 
.0456 
.0726 

%  BaCh 

Sp.  gr.       ||    %  BaCh 

Sp.  gr. 

(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38.  701.) 
BaCl2-fAq  containing  6.94%   BaCl2  has 
sp.  gr.  20°/20°  =  1.0640. 
BaCl2+Aq  containing  11.38%  BaCl2  has 
sp.  gr:  20°/20°  =  1.1086. 
(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  279.) 
Sp.  gr.  of  BaCl2-f-Aq  at  25°. 

8.88 
18.24 

1.0760               27.53 
1.1521       ||       35.44 

1.2245 
1.2837 

(Kremers,  Fogg.  99.  444.) 

Sp.  gr.  of  BaCl2-fAq  at  15°. 

%  BaCh 

Sp.  gr. 

%  BaCh 

Sp.  gr. 

1 

2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 

.00917 
.01834 
.02750 
.03667 
.04584 
.05569 
.06554 
.07538 
.08523 
.09508 
.  10576 
.  11643 
.12711 

14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 

1.13778 
1.14846 
1.15999 
1.17152 
1.18305 
1.19458 
1.20681 
1.21892 
1.23173 
1.24455 
1.25736 
1.27017 

BaCh+Aq 

Sp.  gr. 

1-normal 

Vt"       " 

1.0884 
1.0441 
1.0226 
1.0114 

(Wagner,  Z.  phys.  Ch.  1890,  5.  35.) 
Sp.  gr.  of  BaCl2+Aq. 

t°    |          Concentration  of  BaCh  4-Aq             Sp.    gr. 

25°     1  pt.  BaCl2  in    3.684  pts.  H2O    1.2194 
22.8)  1    "      "      "  52.597     "      "      1.0145 

(Hittorf,  Z 
Temp. 

phys.  Ch.  1902,  39.  628.) 
of  Maximum  Density. 

(Gerlach,  Z.  anal.  8.  283.) 
Sp.  gr.  of  BaCl2+Aq  at  21.5°. 

Weight  of  BaCh  „ 
in  1000  grams  J 
H2O 

""emp.  of  maximum 
density 

Molecular  reduc- 
tion of  temp,  of 
M.  D. 

%m?o2+ 

Sp.  gr. 

%  BaCh  + 
2H2O 

Sp.  gr. 

0 
6.73 
10.42 

20.83 
41.72 

3.982° 
3.207° 
2.783° 
1.572° 
—0.843° 

23.94 
23.88 
24.04 
24.04 

1 
2 
3 
4 
5 
6 
7 
8 
•      9 
10 
11 
12 
13 
14 
15 

1.0073 
1.0147 
.0222 
.0298 
.0374 
.0452 
.0530 
.0610 
.0692 
.0776 
.0861 
.0947 
.1034 
.1122 
.1211 

16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 

1.1302 
1.1394 
1.1488 
.1584 
.1683 
.1783 
.1884 
.1986 
.2090 
1.2197 
1.2304 
1.2413 
1.2523 
1.2636 
1.2750 

(De  Coppet,  C.  R.  1897,  126.  533.) 

BaCl2+Aq  containing  10%  BaCl2  boils  at 
100.6°.    (Gerlach.) 
BaCl2+Aq  containing  20%  BaCl2  boils  at 
101.9°.    (Gerlach.) 

B.-pt.  of  BaCl2+Aq  containing  pts.  BaCl2  to 
100  pts.  H2O.     G  =  according  to  Gerlach 
(Z.  anal.  26.  443)  :  L  =  according  to  Legrand 
(A.  ch.  (2)59.452). 

B.-pt. 

G 

L 

(Schiff,  calculated  by  Gerlach,  Z.c.) 
Sp.  gr.  of  BaCl2+Aq  at  18°. 

100.5° 
101.0 
101.5 
102.0 
102.5 
103.0 
103.5 
104.0 
104.4 
104.5 

6.4 
12.7 
19.0 
25.3 
31.6 
37.7 
43.7 
49.5 

55'.2 

11.0 
19.6 
26.2 
32.5 
38.6     • 
44.5 
50.3 
56.0 
60.1 

%  BaCh 

Sp.  gr. 

%  BaCh 

Sp.  gr. 

5 
10 
15 

1.0445 
1.0939 
1.1473 

20 
24 

1.2047 
1.2559 

(Kohlrausch,  W.  Ann.  1879.  1.) 

BARIUM  CHLORIDE 


83 


Less  sol.  in  H2O  containing  HC1  than  in 
pure  H20,  and  scarcely  sol.  in  cone.  HCl+Aq. 
(Berzelius.) 

Solubility  of  BaCl2  in  HCl+Aq  at  0°. 
BaCl2=no.  %  mols.  (in  milligrammes)  dis- 
solved in  10  cc.  of  the  liquid ;  HCl  =  no.  mols. 
(in  milligrammes)  contained  in  the  same 
quantity  of  liquid. 

Sp.  gr. 

1.250 
1.242 


BaCl2 

HCl 

Sum  of  mols. 

29.45 

0 

29.45 

27.8 

1.1 

28.9 

26.075 

2.8 

28.875 

23.4 

5.0 

28.4 

14.0 

14.36 

28.36 

10.2 

18.775 

28.975 

6.67 

22.75 

29.42 

2.74 

32.0 

34.74 

0.29 

50.5 

50.79 

228 
210 
143 
118 
099 
079 


1.088 


(Engel,  Bull.  Soc.  (2)  45.  653.) 

Sol.  in  about  8000  pts.  cone.  HCl+Aq. 

Sol.  in  about  20,000  pts.  cone.  HCl+Aq 
through  which  HCl  gas  was  passed. 

Practically  insol.  in  cone.  HCl+Aq  con- 
taining Ve  vol.  ether.  (Mar,  Sill.  Am.  J.  143. 

Solubility  in  HCl+Aq  at  30°. 


Composition  of  the 
solution 

Solid  phase 

%by 

wt;  HCI 

%  by  wt. 
BaCh 

0 
5.94 
11.55 
18.11 
32.35 
37.34 
38.63 

27.6 

12.97 

3.85 
0.46 
0.00 
0.00 
0.00 

BaCl2,  2H2O 
it 

(t 
ii 
n 

BaCl2,  2H,O+BaCl2,  H2O 
BaCl2,  H2O 

(Schreinemakers,  Z.  phys.  Ch.  1909,  68.  89.) 

Much  less  sol.  in  HNO3+Aq  than  in  H2O, 
because  Ba(NO3)2  is  nearly  insol.  therein. 
(Wurtz.) 

BaCl2  is  sol.  in  about — 

4.00  pts.  H2O. 

5.00  pts.  NH4OH+Aq  (cone.). 

5.33  pts.  NH4OH+Aq  (1  vol.  cone.:  3  vols. 
H20). 

5.33  pts.  HCl+Aq  (1  vol.  cone.:  4  vols. 
H20). 

8.00  pts.  HC2H3O2+Aq  (1  vol.  commercial 
acid:  1  vol.  H2O). 

6.00  pts.  NH4Cl+Aq  (1  pt.  NH4C1  :  10  pts. 
H2O). 

6.00  pts.  NH4C2H3O2+Aq  (dil.  NH4OH  + 
Aq  neutralized  by  dil.  HC2H3O2+Aq.) 

6.67  pts.  NaC2H3O2+Aq  (commercial 
HC2H3O2  neutralized  by  Na2CO3,  and  dil. 
with  4  vols.  H2O).  ' 

6.33  pts.  Cu(C2H3O2)2+Aq.  See  Stolba  (Z. 
anal.  2.  390). 

5.67  pts.  grape  sugar  (1  pt.  grape  sugar: 
10  pts.  H2O).  (Pearson,  Zeit.  Chem.  1869. 
662.) 


BaCl2+NH4Cl.    Solubility  of  BaCl2 
NH4Cl+Aq  at  30°. 

in 

Composition  of  the 

Solid  phase 

solution 

%  NEUC1 

%  BaCh 

0 

27.6 

BaCl2.2H2O 

5.71 

22.16 

n 

10.06 

18.36 

(( 

13.84 

15.42 

t( 

20.00 

10.89 

tt 

24.69 

8.33 

tc 

25.79 

7.95 

BaCl2.2H2O+NH4Cl 

26.06 

7.99 

tt 

27.47 

3.56 

NH4C1 

29.5 

0 

K 

(Schreinemakers,  Z.  phys.  Ch.  1909,  66. 

688.) 

See  also  under  Ammonium  chloride. 

BaCl2+Ba(OH)2.    Solubility  of  BaCl 
BaO+Aqat30°. 

2  in 

Composition  of 

Solid  phase 

the  solution 

%by 

%by 

wt. 

wt. 

BaO 

BaCh 

0 

27.6 

BaCl2,  2H2O 

1.78 

27.42 

« 

1.79 

27.31 

BaCl2,  2H20+BaCl(OH),  2H20 

1.75 

27.41 

a 

2.33 

24.98 

BaCl(OH),  2H20 

2.50 

24.20 

3.27 

21.46 

4  67 

19.18 

4.86 

18.97 

BaCl(OH),  2H  O+BaO,  9H2O 

4.29 

18.83 

4.64 

18.77 

4.65 

18.10 

4.62 

18.04 

BaO,  9H2O 

4.60 

17.08 

4.58 

12.81 

4.45 

10.77 

4.99 

0 

Sol.  in  CuCl2,NH4Cl+Aq  at  30°.  (Schreine- 
makers, Z.  phys.  Ch.  1909,  66.  688.) 

The  solubility  data  for  the  system  BaCl2+ 
}uCl2 +KC1 + Aq  have  been  determined  at  40 
id  6ot  (Schreinemakers,  C.  C.  1915, 1.  933.) 


BaCl2+HgCl2.     Solubility  of  BaCl2+ 
HgCl2  in  H2O. 


Cms.  per  100  g. 

solution 

Solid  phase 

BaCb 

HgCh 

10.4° 

23.58 

50.54 

BaCl2,2H2O+HgCl2 

10.4 

23.44 

50.74 

10.4 
10.4 

22.58 
22.48 

51.23 
51.41 

BaCl2,3HgCl2,  6H20 

10.4 

22.10 

51.66 

10.4 
25.0 

21.64 
23.02 

51.74 
54.83 

BaCl2,2H2O+HgCl2 

(Foote  and  Bristol,  Am.  Uh.  J.  32.  -24s.; 

84 


BARIUM  CHLORIDE 


Solubility  of  BaCl2+HgCl2  in  H20. 


Temp.  =30 

Temp.  =0° 

%  HgCh 

%  BaCh 

Solid  phase 

%  HgCh 

%  BaCh 

Solid  phase 

0 

27.77 

BaCl2.2H2O 

0 

23.70 

BaCl2.2H20 

2.90 

27.56 

* 

14.25 

24.0 

" 

7.09 

27.47 

* 

36.20 

24.89 

.  " 

12.98 

26.99 

< 

46.12 

24.07 

BaCl2,  3HgCl2.6H2O  + 

22.61 

26.89 

' 

46.05 

24.03 

"    BaCl2.2H2O 

34.57 

26.69 

' 

46.07 

24.05 

M 

46.50 

25.22 

' 

46.59 

23.28 

BaCl2,  3HgCl2.6H20 

55.16 

23.46 

HgCl2+BaCl2.2H2O 

47.78 

21.05 

a 

55.32 

23.08 

H 

48.43 

20.64- 

BaCl2,  3HgCl2.6H20+HgCl2 

55.19 

22.98 

It 

48.49 

20.71 

u 

48.97 

17.87 

HgCl2 

44.33 

18.50 

HgCl2 

41.30 

14.26 

« 

29.0 

11.59 

u 

27.62 

8.41 

« 

16.36 

6.11 

u 

14.19 

7£**7 

2.65 

a 
ft 

3.95 

0 

tt 

.67 

Temp.  =40° 

56.57 

22.98 

BaCl2.2H2O+HgCl2 

(Schreinemakers,  Ch.  Weekbl.  1911,  7.  202.) 
BaCl2+KCl.    Sol.insat.KCl+Aq,  at  first    10°  Pts-  H2°  dissolve,  when  both  salts  are 


without  pptn.  The  KC1  is  pptd.  after  a  time 
until  a  state  of  equilibrium  is  reached. 

100  pts.  H2O  at  16.6°  dissolve  33.8-27.2  pts. 
KC1  and  18.2-34.9  pts.  BaCl2.  (Kopp,  A.  34. 
267.) 

100  g.  sat.  solution  of  BaCl2+KCl  contain 
13.83  g.  BaCl2  and  18.97  g.  KC1  at  25°. 
(Foote,  Am.  Ch.  J.  32.  253.) 


in  excess — 


i 

2 

3 

4 

5 

6 

NaCl    . 
BaCl,  .     .     . 

35.9 

4.1 
34.5 

ss!6 

40.4 

35.3 
19.4 

60'.3 

38.6 

54.7 

BaCl2+Ba(NO3)2. 
Ba(NO3)2+Aq. 


BaCl2   is   sol.  in  sat. 


Solubility  of  BaCl2+Ba(NO»)2  in  H20.  Both 
salts  present  in  solid  phase. 


1,  2,  and  3  are  at  17°.    ( Kopp,  A.  34.  268.) 
4,  5,  and  6  are  at  b.-pt.    (Mulder.) 

Solubility  of  BaCl2+NaCl. 

100  pts.  H2O  dissolve  pts.  BaCl2  and  NaCl 

at  t°. 


t° 

0 
20 
40 
60 

Gms.  per  100  gms. 
solution 

t° 

Gms.  per  100  gms. 
solution 

BaCh 

Ba(NO3)2 

BaCh 

Ba(NO3)2 

22.5 
24.5 
26.5 

28.5 

4.3 
6.0 
7.5 
9.5 

100 
140 
180 
210 

31 
32 
33 

32 

14 
20 
26 
32 

(Etard,  A.  Ch.  (7)  2.  535.) 

Very  slowly  sol.  in  sat.  NaNO3+Aq  with 
separation  of  Ba(NO3)2. 

Rapidly  sol.  in  sat.  KNO3+Aq,  forming 
Ba(NO3)2,  which  separates  out.  (Karsten.) 

BaCl2+NaCl.  BaCl2  is  sol.  in  NaCl+Aq 
at  first  without  separation  of  NaCl,  which, 
however,  finally  separates. 


t< 

Pts. 
BaCl2 

Pts. 
NaCl 

t° 

Pts. 
BaCh 

Pts. 
NaCl 

10 
20 
30 
40 
50 

4.1 
4.1 
5.0 
6.3 

7.9 

33.9 
33.8 
33.7 
33.6 
33.5 

60 
70 
80 
90 
100 

9.7 
11.7 
13.9 
15.9 
17.9 

33.5 
33.6 
33.6 
33.6 
33.6 

(Precht  and  Wittgen,  B.  14.  1667.) 
Solubility  of  BaCl2+NaCl  in  HCl+Aq  at  30°. 

Solid  phase,  NaCl 

Solid  phase,  BaCl2+2H2O 

Sp.  gr. 
of  sat. 
solution 

G.  mol.  litre 

Sp.  gr. 
of  sat. 
solution 

G.  mol.-litre 

HC1 

NaCl 

HC1 

BaCh 

1.2018 
1.1906 
1.1801 
1.1633 
1.1512 
1  .  1427 
1  .  1289 
1.1188 
1.1258 

0.0000 
0.4575 
0.969 
1.786 
2.412 
3.052 
4.152 
5.950 
7.205 

5.400 
4.932 
4.386 
3.589 
2.978 
2.463 
1.628 
0.630 
0.268 

1.3056 
1.2651 
1.2147 
1.1789 
1.1419 
1  .  1068 
1.0880 
1.0895 
1.1024 
1  .  1609 

0.0000 
0.4709 
1.107 
1.622 
2.234 
3.041 
3.953 
3.059 
6.234 
10.25 

1.745 
1.468 
1.122 
0.861 
0.592 
0.307 
0.124 
0.020 
0.00 
0.00 

(Masson,  Chem.  Soc.  1911,  99.  1136.) 

BARIUM  CHLORIDE 


85 


Solubility  of  BaCl2+NaClin  HCl+Aq  at  30°. 


%HC1 

%NaCl 

%BaCl2 

Solid  phase 

0 
4.84 
12.02 
17.20 
23.16 
28.66 
36.51 

23.85 
18.07 
9.55 
4.65 
1.54 
0.47 
0.12 

3.8 

2.27 
0.82 
0.29 
0.00 
0.00 
0.00 

NaCl,BaCl2.2H20 
NaCl+BaCl2.H20 

(Schreinemakers,  Arch.  Neer.  Sc.  ex.  nat.  (2) 
15.  91.) 


,.      (Franklin,  Am.  Ch. 


Insol  in  liquid 
J.  1898,  20.  827.) 

Solubility  in  alcohol:  100  pts.  alcohol  of  given  sp.  gr. 
dissolve  pts.  of  the  anhydrous,  and  crystallized 
salt. 


Sp.  gr. 

Pts. 
BaCh 

Pts. 
BaCl24-2H2O 

0.900 
0.848 
0.834 
0.817 

1.00 
0.29 
0.185 
0.09 

1.56 
0.43 
0.32 
0.06 

(Kirwan.) 

Insol.  in  abs.  alcohol,  or  below  19°  in  al- 
cohol of  over  91%.  Dil.  alcohol  dissolves  less 
BaCl2  than  corresponds  to  the  amount  of  H2O 
present.  (Gerardin,  A.  ch.  (4)  5.  142.) 

Solubility  in  100  pts.  alcohol  at  t°.    D  =sp.  gr. 
of  alcohol;  S=  solubility. 


D  =0.9904 

D  =0.9848 

D  =0.9793 

D  =0.9726 

t° 

s 

t° 

s 

t° 

s 

t° 

.s 

14 
25 
32 

47 
60 

29.1 
32.0 
33.5 
37.4 
39.8 

14 
32 
39 
50 
63 

25.0 
29.1 
30.9 
33.2 
37.6 

11 
15 
20 
35 
45 

19.6 
20.4 
21.7 
24.6 
26.8 

15 
23 
33 
50 

15.6 
17.0 
19.1 
22.0 

D  =0.9573 

D  =0.9390 

D  =0.8967 

D  =0.8429 

t° 

s 

t° 

s 

t° 

s 

t° 

s 

13 
24 
34 
39 
50 

10 
11.4 
12.9 
13.8 
15.2 

12 
23 
31 
37 

47 

6.5 
7.2 
8.3 
9.0 
10.1 

12 
30 

47 

0.1 
4.3 

4.9 

12 
19 
25 
50 
67 

0.00 
0.00 
0.04 
0.28 
0.377 

(Gerardin,  A.  ch.  (4)  5.  142.) 

Solubility  in  dil.  alcohol  of  x%  by  weight 
at  15°. 

%  alcohol  0         10       20       30      40     60    80 

Pts.  BaCU,  2H2O  30.25  23.7  18.0  12.8  9.3  3.4  0.5 

(Schiff,  A.  118.  365.) 

Sol.  in  6885-8108  pts.  99.3%  alcohol  at 
14.5°,  and  in  1857  pts.  at  ebullition.  (Frese- 
nius.) 


Solubility  of  BaCl2  in  alcohol  +Aq. 

t 

alcohol 

Cr/ 

BaCb 

Solid  phase 

30° 

0 

32.67 
50.16 
66.72 
92.53 
94.83 
94.75 
94.60 
97.14 
98.17 
99.41 

27.95 
10.63 
5.68 
2.23 
0.05 
0.07 
0.05 
0.07 

'6^08 

BaCl2.2H2O 
ii 

ii 
ii 

« 

BaCl2.2H20+BaCl2.H20 

<(               .  • 
t( 

BaCl2.H2O 
BaCl2.H2O+BaCl2 
BaCl2 

60° 

0 

16.68 
34.10 
66.02 
88.55 
90.11 
90.39 
93.95 

31.57 
20.16 
13.21 

2.82 
0.25 
0.09 

BaCl2.2H2O 

u 
II 
(t 

n 

BaCl2.2H20+BaCl2.H20 

ti 

BaCl2.H2O 

..... 

(Schreinemakers  and  Massink,  Chem. 
Weekbl.  1910,  7.  213.) 

100  pts.  absolute  methyl  alcohol  dissolve 

2.18  pts.  BaCl2  at  15.5°,  and  7.3  pts.  BaCl2, 

2H2O  at  6°.    (de  Bruyn,  Z.  phys.  Ch.  10.  783.) 

At  15°  C.     1  pt.  by  weight  is  sol.  in:— 

78  pts.  methyl  alcohol  of  sp.  gr.  0.790 
7,000   "     ethyl         "        "    "    "  0.8035 
100,000   "     propyl       "        "     "     "  0.8085 
(Rohland,  Z.  anorg.  1897,  15.  413.) 

Absolutely  insol.  in  boiling  amyl  alcohol. 
(Browning,  Sill.  Am.  J.  144.  459.) 

Absolutely  insol.  in  acetic  ether.  (Cann. 
C.  R.  102.  363.) 

Very  si.  sol.  in  acetone.  (Krug  and  M'El- 
roy,  J.  Anal.  Ch.  6.  184.) 

100  pts.  by  weight  of  glycerine  dissolve  10 
pts.  BaCl2  at  15.5°.  (de  Bruyn,  Z.  phys.  Ch. 
10.  783.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.)  (Eidmann,  C.  C.  1899,  II.  1014.) 

Insol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1370.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Insol.  in  anhydrous  pyridine,  97%  pyri- 
dine+Aq.  and  95%  pyridine  -f  Aq.  SI.  sol. 
in  93%  pyridine +Aq.  (Kahlenberg,  J.  Am. 
Chem.  Soc.  1908,  30.  1107.) 

+H2O.  Solution  of  monohydrate  sat.  at  6° 
contains  31.57%  BaCl2.  (Schreinemakers, 
Chem.  Weekbl.  1910,  7.  213.) 

2.5  grams  of  the  monohydrate  are  sol.  in 
100  cc.  of  methyl  alcohol  at  14°.  (Kirschner, 
Z.  phys.  Ch.  1911,  76.  176.) 

Exact  solubility  in  methyl  alcohol  cannot 
be  determined  as  BaCl2+H2O  separates  out 
from  a  sat.  solution  of  the  dihydrate.  (Kirsch- 
ner, Z.  phys.  ch.  1911,  76.  177.) 

Barium    cadmium    chloride,    BaCl2,CdCl2  + 

4H2O. 
Easily  sol.  in  H2O.    (v.  Hauer.) 


BARIUM  MERCURIC  CHLORIDE 


Solubility  in  H2O  at  t°. 


t- 

100  pts.  solution  contain  pts. 

100  g.  of 
solution 
contain  g.  salt 

100  g.  H2O 
dissolve 
g.  salt 

100  mols.  H20 
dissolve  mols.  of 
anhydrous  salt 

Cl 

Ba 

Cd 

22.5 

15.19 

14.71 

11.98 

41.88 

72.06 

3.32 

32.9 

16.18 

16.09 

12.40 

44.59 

80.73 

3.72 

41.4 

16.95 

16.81 

13.05 

46.87 

88.01 

4.06 

53.4 

18.21 

18.13 

13.95 

50.30 

101.21 

4.66 

62.0 

18.81 

18.74 

14.73 

52.28 

109.56 

5.05 

97.8 

22.48 

22.00 

17.57 

62.05 

163.50 

7.53 

108.3 

23.51 

22.79 

18.53 

64.83 

184.33 

8.49 

109.2 

23.69 

29.95 

18.67 

65  .,31 

188.27 

8.67 

(Rimbach,  B.  1897,  30.  3083.) 

BaCl2.2CdCl2+5H2O.    Quite  difficultly  sol.  in  H2O.    (v.  Hauer.) 

Solubility  in  H20  at  t°. 


t° 

100  pts.  by  wt.  of  solution  contain  pts.  by  wt. 

100  g.  of 
solution 
contain  g.  salt 

100  g.  H2O 
dissolve 
g.  salt 

100  mols.  H20 
dissolve  mols.  of 
anhydrous  salt 

Cl 

Ba 

Cd 

22.6 
41.3 
53.9 
62.2 
69.5 
107.2 
107.2 

16.89 
18.15 
18.78 
19.66 
20.18 
23.31 
23.16 

11.00 
11.77 
12.41 
12.83 
13.09 
14.87 
14.93 

17.71 
19.22 
19.85 
20.59 
21.20 
24.11 
24.39 

45.60 
49.14 
51.04 
53.08 
54.47 
62.29 
62.48 

83.82 
96.62 
104.25 
113.13 
119.64 
165.18 
166.53 

2.63 
3.03 
3.27 
3.55 
3.76 
5.19 
5.23 

(Rimbach,  B.  1897,  30.  3083.) 


Barium  mercuric  chloride,  basic,  BaCl2,  HgO 

+6H2O. 
Decomp.  by  H20.    (Andre,  C.  R.  104.  431.) 

Barium  mercuric  chloride,  BaCl2,  2HgCl2  + 
2H2O. 

Efflorescent  in  dry  air;  sol.  in  H2O.  (v, 
Bonsdorff,  Pogg.  17.  130.) 

The  salt  BaCl2,  2HgCl2+2H2O  described  by 
Bonsdorff  does  not  form  under  the  conditions 
which  he  gives.  (Foote,  Am.  Ch.  J.  1904,  32. 
251.) 

BaCl2,3HgCl2+6H2O.  Solubility  deter- 
minations with  mixtures  of  BaCl2  and  HgCl 
show  that  these  chlorides  do  not  form  a  double 
salt  at  25°,  but  that  a  transition  temp,  exists 
at  about  17.2°  below  which  the  salt  BaCl2, 
3HgCl2+6H2O  forms.  (Foote,  Am.  Ch.  J. 
1904,  32.  251.) 

+8H2O.  Less  sol.  in  H20  than  the  Sr  and 
Mg  double  salts.  (Swan,  Am.  Ch.  J.  1898,  20. 
633.) 

Barium  rhodium  chloride,  3BaCl2,  Rh2Cl6. 
See  Chlororhodite,  barium. 

Barium  stannous  chloride,  BaCl2,   SnCl2  + 
4H20. 

Sol.  in  H2O.    (Poggiale,  C.  R.  20.  1183.) 
Barium  stannic  chloride. 

See  Chlorostannate,  barium. 

Barium  uranium  chloride,  BaCl2,UCl4. 

Decomp.  by  H2O.  (Aloy,  Bull.  Soc.  1899, 
(3)  21.  265.) 


Barium  zinc  chloride,  BaCl2,  ZnCl2+4H2O. 

Deliquescent,  and  sol.  in  H2O.  (Warner, 
C.  N.  27.  271.) 

Pptd.  from  warm  solution  only.  (Ephraim, 
Z.  anorg.  1910,  67.  381.) 

+2^H2O.  Pptd.  from  cold  solution. 
(Ephraim.) 

Barium  chloride  hydrazine,  BaCl2,  2N2H4. 

Hydroscopic.  (Franzen,  Z.  anorg.  1908, 
60.  290.) 

Barium  chloride  hydroxylamine,  BaCl2, 

2NH2OH. 

Very  sol.  in  H2O.  (Crismer,  Bull.  Soc.  (3) 
3.  118.) 

Barium  chloride  sulphuric  anhydride,  BaCl2, 

2S03. 

Decomp.  by  H2O.  (Schultz-Sellack,  B.  4. 
113.) 

Barium  chlorofluoride,  BaClF. 

Difficultly  sol.  in  H2O,  but  much  more  sol. 
than  BaF2.  Decomp.  by  H2O,  so  that  when 
washed  on  filter,  the  nitrate  contains  more 
BaCl2  than  BaF2.  (Berzelius,  Pogg.  1.  19.) 

Insol.  in  and  undecomp.  by  boiling  alcohol; 
sol.  in  cone.  HC1  and  HNOs.  Decomp.  by 
hot  H20,  hot  H2SO4,  dil.  acetic  acid,  dil.  HC1 
or  dil.  HNO3.  (Defacqz,  C.  R.  1904,  138. 

Barium  cyanamide,  BaCN2. 

Decomp.  by  H2O.    (Frank,  C.  C.  1902,  II. 

774.) 


BARIUM  HYDROXIDE 


87 


Barium  sw&fluoride   sodium   fluoride,   BaF, 

NaF. 

Decomp.  by  H2O.  (Guntz,  C.  R.  1903, 
136.  750.) 

Barium  fluoride,  BaF2. 

Scarcely  sol.  in  H2O  (Berzelius) ;  less  sol.  in 
H2O  than  CaF2. 

1  liter  H2O  dissolves  1630  mg.  BaF2  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1904,  60.  356.) 

1605  mg.  are  contained  in  1  1.  of  sat.  solu- 
tion at  18°.  (KohJrausch,  Z.  phys.  Ch.  1908, 
64.  168.) 

Insol.  in  molten  MnCl2,  MnBr2,  MnI2, 
MnCl2+BaCl2,  MnBr2+BaBr2  and  MnI2+ 
BaI2.  (Defacqz,  A.  ch.  1904,  (8)  1.  350.) 

Easily  sol.  in  HC1,  HNO3,  or  HF+Aq. 
(Gay-Lussac  and  Thenard.) 

SI.  sol.  in  liquid  HF.  (Franklin,  Z.  anorg. 
1905,  46.  2.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

Sol.  in  an  aqueous  solutio'n  of  sodium  cit- 
rate. (Spiller.) 

Barium  tin  (stannic)  fluoride. 
See  Fluostannate,  barium. 

Barium  tellurium  fluoride,  BaF2,  2TeF4. 

Decomp.  by  H2O.  (Hogbom,  Bull.  Soc.  (2) 
35.  60.) 

Barium  titanium  fluoride. 
See  Fluotitanate,  barium. 

Barium  titanyl  fluoride,  TiO2F2,  BaF2. 

See  Fluoxypertitanate  and  fluoxytitanate, 
barium. 

Barium  uranyl  fluoride. 
See  Fluoxyuranate,  barium. 

Barium  vanadyl  fluoride. 
See  Fluoxyvanadate,  barium. 

Barium  zirconium  fluoride,  3BaF2,  2ZrF4  + 

2H2O. 

Insoluble  precipitate.    (Marignac.) 
See  also  Fluozirconate,  barium. 

Barium  fluoiodide,  BaF2,  BaI2. 

Decomp.  by  H2O,  dil.  HC1,  dil.  HNO3  or 
hot  H2SO4.  Sol.  in  HI  and  HNO3.  Insol. 
in  and  undecomp.  by  boiling  alcohol.  De- 
comp. by  dil.  acetic  acid.  (Defacqz,  C.  R. 
1904,  138.  199.) 

Barium  hydride,  BaH. 

Decomp.  by  H2O  or  HCl+Aq.  (Winkler, 
B.  24.  1979.) 

Decomp.  by  H20.  (Guntz,  C.  R.  1901, 
132.  964.) 

Barium  hydrosulphide,  BaS2H2. 

Easily  sol.  in  H2O.    Insol.  in  alcohol. 

+4H2O.  Sol.  in  H20,  and  the  solution  dis- 
solves S.  (Veley,  Chem.  Soc.  49.  369.) 


100  pts.  H2O  dissolve  pts.  BaO  at  t°. 

"t 

Pts.  BaO 

t° 

Pts.  BaO 

t° 

Pts.  BaO 

0 
5 
10 
15 
20 
25 

1.5 
1.75 
2.22 

2.89 
3.48 
4.19 

30 
35 
40 
45 
50 
55 

5.0 
6.17 
7.36 
9.12 
11.75 
14.71 

60 
65 
70 
75 

80 

18.76 

24.67 
31.9 
56.85 
90.77 

Barium  hydroxide,  BaO2H2. 

100  pts.  cold  H2O  dissolve  5  pts.  BaO2H2. 
boiling  50 

(Davy.) 
100  pts.  H2O  at  20°  dissolve  3.45  pts.  BaO. 

(Bineau,  C.  R.  41.  509.) 
100  pts.  H2O  at  13°  dissolve  2.86  pts.  BaO. 
47°        "      13.3 
70°        "      17.9 
(Osann.) 


(Rosenthiel  and  Ruhhnann,  J.  B.  1870.  314.) 
100  pts.  H2O  dissolve  at  25°  55.08  millimols. 
Ba°22H2>     (Herz  and  Knoch,  Z.  anorg.  1904, 
41.  315.) 

Sp.  gr.  of  BaO2H2+Aq. 


%BaO 

Sp.  gr. 

%BaO 

Sp.  gr. 

30 
19 
2.6 

1.6 
1.3 
1.03 

1.8 
0.9 

1.02 
1.01 

(Dalton.) 


Sp.  gr.  of  Ba02H2-f  Aq  at  18°  containing 
1.25%  BaO2H2  =  1.0120;  containing  2.5%  = 
1.0253.  (Kohlrausch,  W.  Ann.  1879,  6.  41.) 

Sp.  gr.  of  BaO2H2+Aq  at  80°. 


Sp.  gr. 

% 

BaO2H2 
by 
volume 

BaOzHz 
by 
weight 

Sp.  gr. 

% 
Ba02H2 
by 
volume 

% 

BaO2H8 
by 
weight 

.514 

58.22 

38.45 

1.219 

24.53 

20.12 

.500 

56.31 

37.54 

1.200 

23.00 

19.17 

.479 

54.14 

36.60 

1.195 

22.15 

18.53 

.458 

49.38 

33.87 

1.174 

19.83 

16.89 

.450 

48.90 

33.72 

1.152 

17.78 

15.43 

.413 

45.99 

32.55 

1.129 

16.01 

14.18 

.400 

45.00 

32.14 

1.125 

15.80 

14.04 

.390 

44.22 

31.81 

1.114 

14.56 

13.07 

1.375 

42.40 

30.84 

1.100 

13.06 

11.87 

1.368 

41.45 

30.30 

1.076 

10.58 

9.83 

1.350 

38.60 

28.59 

1.062 

9.16 

8.62 

1.338 

37.30 

27.88 

1.049 

7.55 

7.20 

1.312 

35.02 

26.69 

.040 

6.51 

6.26 

1.301 

34.02 

26.13 

.031 

5.18 

5.02 

1.278 

31.48 

24.67 

.022 

4.78 

4.67 

1.249 

28.14 

22.52 

.015 

3.90 

3.84 

1.236 

26.41 

21.36 

.009 

3.37 

3.34 

(Haff,  C.  N.  1902,  86.  284.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

More  sol.  in  NaCl+Aq,  KNO3+Aq,  or 
NaNO3+Aq  than  in  H2O.  (Karsten.) 

Not  precipitated  by  alcohol. 


88 


BARIUM  HYDROXIDE 


Sol.  with  combination  in  absolute  alcoho 

J                 1          -]„_.,,           J-l  1        -1--T--1               T  1          i_ 

B.-pt.  of  Ba02H2.8H2O+Aq,  etc.—  Continued. 

and   anhydrous 
ether. 

meunyi    aiuonoi.      iiisoi.    m 

Bpt. 

Time 

%BaO 

Insol.  in  acetone.     (Naumann,  B.  1904,  37. 

108 

19' 

e;7  40 

4329;  Eidmann, 

C.  C.  1899,  II.  1014.) 

JLUO 

108.5 

JL0 

U  i    .  Ttt7 

58.74 

SolubHity 

in  acetone  +Aq  at  25°. 

109 

13' 

61.44 

A  =  cc.   acetone  in   100  cc. 

acetone  -f-Aq 

109 

17'  40" 

63.65 

Ba02H2        „ 

imols.  Ba02H 

2  in  100  cc.  of 

108 
105 

17'  50" 

18' 

66.53 
67.51 

2 

the  solution. 

100 

18'  45" 

68.17 

S  =  sp.  gr.  of  the  solution. 

(Bauer,  Z.  anorg.  1905,  47.  407.) 

A 

BaO2H2 

s 

Solubility  in  Ba(N03)2+Aq  at  25°. 

2 

Solution  sat.  with  respect  to  both  Ba(NOa)2 

0 

55.08 

1.04790 

and  BaO2H2,  8H2O. 

10 

31.84 

1.01677 

_      _. 

20 
30 

A  f\ 

17.79 
9.10 

0.99268 
0.97630 

Sp.  gr.  25°/25° 

g.  .03,0  £is 
Ba(OH)2in 
100  g.  H2O 

g.  Ba  (NOs)s  in 
100  g.  H2O 

40 
50 

4.75 
1.54 

0.95605 
0.93980 

1.1448 

5.02 

11.48 

60 

0.48 

0.91790 

1.1371 

.       4.93 

10.21 

70 

0.08 

0.89562 

1.1288 

4.83 

8.66 

1  .  1220 

4.72 

7  55 

(Herz,  Z. 

anorg.  1904,  41.  321.) 

1.1133 

4>2 

7^01 

BaO2H2  is  sol.  in  an  aqueous  solution  of 
cane  sugar  (Hunton,  Phil.  Mag.  (3)  11.  156)  ; 
also  in  an  aqueous  sol.  of  mannite  (Favre,  A. 
ch.  (3)  11.  76);  sorbine  (Pelouze);  hot  solu- 
tion of  quercite,  separating  on  cooling  (Des- 

1.1062 
1.1044 
1.1010 
1.0975 
1.0949 
1.0937 

4.65 
4.61 
4.64 
4.60 
4.55 
4.54 

6.82 
6.55 
6.08 
5.66 
5.46 
5.32 

saignes)  . 
+3H2O.    Decomp.  by  H2O  free  from  car- 
bonic acid.     SI.  sol.  in  alcohol  and  ether. 
(Bauer,  Z.  anorg.  1905,  47,  416.) 
Solubility  in  H2O  the  same  as  that  of  the 
comp.  with  8H2O.    Insol.  in  alcohol  and  ether. 
(Bauer,  Zeit.  angew.  Ch.  1903,  17.  341.) 
Nearly  insol.  in  alcohol  and  ether.    (Bauer, 
Zeit.  angew.  Ch.  1903,  16.  349.) 

1.0885 
1.0864 
1.0840 
1.0790 
1.0774 
1.0731 
1.0711 
1.0651 

1/~l£SO/j 

4.52 
4.53 
4.52 
4.48 
4.46 
4.40 
4.42 
4.35 

4.44 
4.41 
4.04 
3.47 
3.14 
2.79 
2.53 
1.88 

+8H2O.    Sol.  in  20  pts.  cold,  and  3  pts. 
boiling  H20   (Graham);   17.5  pts.   H2O   at 
15.5°,   and  in  all  proportions  of  hot  H2O. 
(Hope.)    Sol.  in  19  pts.  H2O  at  15°,  and  2  pts. 

.UO.JD 
1.0640 
1.0538 
1.0512 

4!35 
4.29 
4.29 

1A5 
0.43 
0 

at  100°.    (Wittstein.) 
If  Ba02H2+8H20  is  heated  it  dissolves  in 
the  crystal  H2O  and  the  solution  has  the 

(Parsons  and  Corson,   J.   Am.   Chem.   Soc. 
1910,  32.  1385.) 

following  bpts. 
%BaO    49.05 
B.-pt.       103° 

50.05        52.43        53.72 
104°           105°           106° 

Solubility  of  Ba(OH)2+8H2O  (solid  phase) 
in  MCl+Aq  (mol.  per  litre  of  solution) 
at  25°. 

%BaO    55.35 

57.49        58.74        61.44 

Solution  of 

(cr)                (OHO 

B.-pt.       107° 

i  n«°         i  n 

»  5°        ina° 

BaO2H2+3H20  separates  at  109°.    (Bauer, 

LiCl 

0                    0.555 

Zeit.  angew.  Ch. 

1903,  17.  345.) 

(( 
ff 

0.75                 0.745 

B.-pt.  of  BaO2H2.8H20+Aq  at  732  mm. 


Bpt. 

Time 

%BaO 

78°  (mpt.) 
78 
103 
104 
105 
106 
107 

0 

4' 
6'  30" 
6'  45" 
7'  30" 
9'  25" 
10'  45" 

48.45 
48.45 
49.05 
50.05 
52.43 
53.72 
55.35 

BARIUM  OXIDE 


89 


Solubility  of  BaO  in  NaOH+Aq  at  30°. 

Barium  iodide,  basic,  Ba(OH)I+9H2O. 

%  Na2O 

%BaO 

Solid  phase 

See  Barium  oxyiodide. 

0 

4.99 

BaO.  9H2O 

Barium  bismuth  iodide,  BaI2,  2BiI3  +  18H2O. 

4.78 

64Q 

1.29 

OCQ 

(( 

Deliquescent;  decomp.  by  H2O.     (Linau, 

.  TrO 

9.63 

.  oy 
0.57 

u 

Pogg.  111.  240.) 

11.62 

0.53 

a 

Barium  cadmium  iodide,  BaI2,  CdI2+5H2O. 

17.87 
23.28 

0.47 
1.06 

a 
(t 

Deliquescent.    (Croft.) 

24.63 

.87 

BaO  .  9H2O  -fBaO  .  4H2O 

Barium  mercuric  iodide,  BaI2,  2HgI2. 

26.14 
27.72 

OQ   4.0 

.84 
.75 

KO 

BaO.  4H2O 

14 

(( 

Decomp.  by  much  H2O.    (Boullay.) 
BaI2,  HgI2.    Sol.  in  H2O.     (Boullay.) 

£o  .  1C 

29.24 
32.12 
34.72 
41.09 

.  Oo 

.34 
0.82 
0.59 
0.57 

Ba0.4H2O+BaO.2H2O 
BaO.2H2O 

a 

BaO.2H2O+NaOH.H2O 

Sp.    gr.     of    sat.     solution  =  3.575-3.588. 
(Rohrbach,  W.  Ann.  20.  169.) 
+5H2O.    (Duboin,  C.  R.  1906,  143.  314.) 
2BaI2,   3HgI2+16H2O.     (Duboin,   C.   R. 
1906,  142.  888.) 

42 

0 

NaOH.H20 

BaI2,  5HgI2+8H2O.    As  the  corresponding 

(Schreinemakers,  Z.  phys.  Ch.  1909,  68.  84.) 
50%  alcohol  dissolves  less  than  0.5%  oJ 

Ca  salt.    (Duboin,  C.  R.  1906,  142.  888.) 
3BaI2,  5HgI2+21H20.    Very  deliquescent. 
(Duboin,  C.  R.  1906,  142.  889.) 

its  wt.  of  BaO2H2+8H2O.     (Beckmann,  J 
pr.  1883,  (2)  27.  138.) 

Barium  sw&iodide  sodium  iodide,  Bal,  Nal, 

Decomp.  by  H20.     (Guntz,  C.  R.  1903, 

136.  750.) 

Barium  iodide,  BaI2. 

Not  deliquescent.     Very  sol.  in  H2O  and 
alcohol.    100  pts.  of  anhydrous  salt  dissolve: 
atO°    19.5°   30°  40°  60°  90°   106° 
in  59     48      44     43     41     37      35  pts.  H2O. 
(Kremers,  Pogg.  103.  66.) 

Sp.  gr.  of  BaI2+Aq  containing: 
5          10        15        20        25        30%BaI2 
1.045  1.091  1.143  1.201  1.265  1.333 

35        40        45        50        55       60%BaI2. 
1.412  1.495  1.596  1.704  1.825  1.970 
(Kremers,  Pogg.  111.  63,  calculated  by  Ger- 
lach,  Z.  anal.  8.  279.) 

Easily  sol.  in  alcohol.    (Henry.) 
SI.    sol.    in   benzonitrile.      (Naumann,    B. 
1914,  47.  1369.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328;  Eidmann,  C.  C.  1899,  II.  1014.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3789.) 

+2H20.  At  15°  C.,  1  pt.  by  weight  in  sol.  in: 

22  pts.  methyl  alcohol  sp.  gr.  0.790 

93    "  "  "        "     "    0.8035 

307   "          "          "        "     "    0.8085 

(Rohland,  Z.  anorg.  1897,  15.  413.) 

+7H2O.    (Thomson,  B.  10.  1343.) 

The  composition  of  the  hydrates  formed 
by  BaI2  at  different  dilutions  is  calculated 
from  determinations  of  the  lowering  of  the 
fr.-pt.  produced  by  BaI2  and  of  the  conduc- 
tivity and  sp.  gr.  of  BaI2+Aq.  (Jones,  Am. 
Ch.  J.  1905,  34.  306.) 


Barium  stannous  iodide. 

Very  sol.  in  H2O.    (Boullay.) 

Barium  zinc  iodide,  BaI2,  2ZnI2. 

Deliquescent,  and  sol.  in  H2O.    (Rammels- 
berg.) 

+4H2O.      Very   hydroscopic.      (Ephraim, 


ery 
,  67. 


Z.  anorg.  1910,  67.  385.) 

Barium  nitride,  Ba3N2. 

Decomp.  H2O  violently,  not  alcohol.  (Ma- 
quenne,  A.  ch.  (6)  29.  219.) 

BaN6. 

See  Barium  azoimide. 

Barium  oxide,  BaO. 

Sol.  in  H2O  with  evolution  of  heat. 

Easily  sol.  in  dil.  HNO3,  or  HCl+Aq. 

Solubility  in  NaOH+Aq.  See  Barium 
lydroxide. 

Solubility  in  Na2O,  HC1,  +H2O  at  30°. 
Schreinemakers,  Z.  phys.  Ch.  1909,  68.  98.) 

Solubility  in  Na2O,  NaCl,  BaCl2+Aq  at 
50°.  (Schreinemakers.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
898,  20.  827.) 

Sol.  with  combination  in  absolute  alcohol 
and  anhydrous  wood-spirit.  Insol.  in  ether. 

Easily  sol.  in  absolute  methyl  alcohol. 

1  1.  absolute  ethyl  alcohol  sat.  with  BaO  at 
9°  contains  213.8  g.  BaO.  (Berthelot,  Bull. 
Soc.  8.  389.) 

Sol.  in  methyl  alcohol.  (Neuberg  and 
STeimann,  Biochem.  Z.  1906,  1.  173.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
I.  1014;  Naumann,  B.  1904,  37.  4329.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
909,  42.  3790.) 

See  also  Barium  hydroxide. 

Jarium  peroxide,  BaO2. 
Insol.  in  H2O;  decomp.  by  boiling  H20. 


90 


BARIUM  OXYBROMIDE 


Sol.  in  acids  with  formation  of  hydrogen 
dioxide. 

Forms  hydrate  with  8H2O;  also  10H2O 
(Berthelot,  A.  ch.  (5)  21.  157);  also  a  com- 
pound BaO2,  H2O2,  which  is  very  unstable,  si. 
sol.  in  cold  H2O,  and  insol.  in  alcohol  or  ether. 
(Schone,  A.  192.  257.) 

+8H2O.  100  cc.  pure  H2O  dissolve  0.168 
g.  BaO2+8H20;  if  H2O  contains  0.3  g. 
Ba(OH)2+8H2O,  only  0.102  g.  BaO2+8H20 
are  dissolved;  if  0.6  g.  Ba(OH)2+8H20  only 
0.019  g.  BaO2+8H2O  are  dissolved.  (Schone, 

A.  1878,  192.  266.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 

Barium  oxybromide,  Ba(OH)Br+2H20. 

Decomp.  by  H2O.  (Beckmann,  J.  pr.  (2) 
27.  132.) 

BaBr2,BaO  +5H2O.  SI.  sol.  in  H2O.  (Tas- 
silly,  C.  R.  1895,  120.  1340.) 

Barium  oxychloride,  Ba(OH)Cl+2H2O. 

Decomp.  by  H2O.  (Beckmann,  J.  pr.  (2) 
26.  388,  474.) 

Barium  mercury  oxychloride,  BaCl2,  HgO-f 

6H20. 
Decomp.  by  H20.    (Andre,  C.  R.  104.  431.) 

Barium  oxyiodide,  Ba(OH)I+9H2O. 

Decomp.  by  H2O  and  alcohol.    (Beckmann, 

B.  14.  2154.) 

BaI2,BaO+9H2O.  SI.  sol.  in  H2O.  (Tas- 
silly,  C.  R.  1895,  120.  1340.) 

Barium  oxysulphides,  Ba;O4S3+58H2O, 

Ba2OS  +  10H2O,  Ba4OS3+28H2O. 
Very  unstable;  decomp.  by  recrystalliza- 
tion  into  BaS2H2  and  BaO2H2. 

Barium  phosphide,  BaP2. 

Decomp.  by  H2O.  (Dumas,  A.  ch.  32. 
364.) 

Ba3P2.  Crystallized.  Sol.  in  dil.  acids; 
insol.  in  cone,  acids;  decomp.  by  H2O.  Insol. 
in  organic  solvents  at  ord.  temp.  (Jaboin, 

C.  R.  1899,  129.  765.) 

Barium  selenide,  BaSe. 
Sol.  in  H2O  with  decomp. 
SI.  sol.  in  H2O.    (Favre,  C.  R.  102.  1469.) 

Barium  silicide,  Ba2Si. 

(Jungst,  C.  C.  1906,  I.  195.) 

BaSi2.  Slowly  decomp.  by  H2O,  not  by 
NH4OH+Aq.  Rapidly  decomp.  by  cone. 
NaOH.  Sol.  in  HNO3,  H2SO4  and  H3PO4 
with  evolution  of  spontaneously  inflammable 
gas.  Sol.  in  HF  and  HC1.  Sol.  in  acetic  acid 
without  evolution  of  gas.  (Moissan,  Traite 
ch.  min.  1904,  III.  680.) 

Decomp.  rapidly  in  both  hot  and  cold  H2O. 
(Bradley,  C.  N.  1900,  82.  150.) 


Barium  sulphide,  BaS. 

Sol.  in  H2O  with  decomp. 

Crystallized.    Decomp.  by  H2O. 

Attacked  by  cold  cone.  HNO3.  (Mourlot, 
A.  ch.  1899,  (7)  17.  521.) 

Cryst.  modification  is  less  readily  acted  on 
by  air  and  other  reagents  than  the  amorphous 
modification;  sol.  in  fuse  oxidizing  agents. 
(Mourlot,  C.  R.  1898,  126.  645.) 

+H2O.  (Neuberg  and  Neimann,  Biochem. 
Z.  1906,  1.  174.) 

+6H2O.  Slowly  sol.  in  boiling  H2O,  with 
decomp.;  insol.  in,  but  decomp.  by  boiling 
alcohol.  (Schone.) 

Barium  sulphide,  Ba4S7+25H2O  (?). 

Sol.  in  H2O.     (Schone,  Pogg.  112.  215.) 

Barium  bisulphide,  BaS3. 

Sol.  in  large  amount  of  boiling  H2O. 
(Schone,  Pogg.  112.  215.) 

Barium  tefrasulphide,  BaS4+H2O. 

Easily  sol.  in  H2O,  especially  if  hot;  sol.  in 
2.42  pts.  H2O  at  15°;  insol.  in  CS2  or  alcohol. 
(Schone,  Pogg.  112.  224.) 

+2H2O.     (Veley,  Chem.  Soc.  49.  369.) 

Barium  pentasulphide,  BaS6. 
Known  only  in  solution. 

Barium  mercuric  sulphide,  BaS,  HgS+5H2O. 
Sol.  in  H2O.    (Wagner,  J.  pr.  98.  23.) 

Barium  nickel  sulphide,  BaS,  4NiS. 

Sol.  in  warm  cone.  HC1.  (Bellucci,  C.  A. 
1909,  293.) 

Barium  stannic  sulphide. 
See  Sulphostannate,  barium. 

Barium    uranyl    sulphide,    6BaS,    U02S  + 


Decomp.  by  HCl+Aq.  (Remele",  Pogg. 
124.  159.)  - 

Baryta. 
See  Barium  oxide,  BaO. 

Beryllium,  Be. 

For  beryllium  and  its  salts,  see  Glucinum 
and  the  corresponding  salts. 

Bismuth,  Bi. 

Not  attacked  by  H20.  Very  slowly  at- 
tacked by  HCl+Aq  (Troost).  Very  si.  sol. 
in  cone.  HCl+Aq  (Schiitzenberger,  Willm). 
Not  attacked  by  dil.  HCl+Aq  (Naquet  and 
Hanriot).  Very  slowly  attacked  by  cold  HC1 
+Aq  (Godeffroy).  According  to  very  careful 
experiments  pure  Bi  is  absolutely  unattacked 
by  hot  or  cold,  dil.  or  cone.  HCl+Aq  except 
in  presence  of  oxygen.  (Ditte  and  Metzner, 
A.  ch.  (6)  29.  397.) 

Not  attacked  by  dil.  H2SO4+Aq.    Decomp. 


BISMUTH  POTASSIUM  CHLORIDE 


91 


by  hot  cone.  H2SO4.  Easily  sol.  in  dil.  or 
cone.  HNO3+Aq,  or  aqua  regia. 

Not  attacked  by  pure  HNO3+Aq  of  1.52  to 
1.42  sp.  gr.  at  20°;  violently  attacked  by  a 
more  dil.  acid,  but  the  acid  becomes  concen- 
trated thereby.  Cone.  HNO3+Aq  attacks 
only  by  heating  or  adding  NO2.  (Millon,  A. 
ch.  (3)  6.  95.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  827.) 

l/2  ccm.  oleic  acid  dissolves  0.0091  g.  Bi  in 
6  days.  (Gates,  J.  phys.  Chem.  1911,  16. 
143.) 

Bismuth  arsenide,  Bi3As4. 
(Descamp,  C.  R.  86.  1065.) 

Bismuth  dibromide,  Bi2Br4. 

Not  known  in  a  pure  state.  (Weber,  Pogg. 
107.  599.) 

Bismuth  inbromide,  BiBr3. 

Very  deliquescent.  Decomp.  by  H2O.  Sol. 
in  alcohol  or  ether. 

Sol.  in  AlBr3.  (Isbekow,  Z.  anorg.  1913, 
84.  27.) 

Bismuth  hydrogen  bromide,  BiBr3,  2HBr+ 
4H2O. 

Deliquescent. 

Decomp.  in  the  air.  (Aloy,  Bull.  Soc.  1906, 
(3)  35.  398.) 

Bismuth  caesium  bromide,  2BiBr3,  3CsBr. 

Ppt.    Insol.  in  HBr. 

Sol.  in  HC1  and  in  HN03.  (Hutchins,  J. 
Am.  Chem.  Soc.  1907,  29.  33.) 

Bismuth  potassium  bromide,  BiBr3,2KBr. 

Decomp.  by  H2O.  (Aloy,  Bull.  Soc.  1906, 
(3)  35.  398.) 

Bismuth  bromide  ammonia,  BiBr3,  3NH3. 

Sol.  in  HCl+Aq. 

BiBrs,  2NH3  (?). 

2BiBr3,  5NH3.  Not  deliquescent;  not  de- 
comp.  by  H2O;  easily  sol.  in  dil.  acids. 
(Muir,  Chem.  Soc.  29.  144.) 

Bismuth  bromide  potassium  chloride, 


Decomp.  by  H2O.    (Atkinson,  Chem.  Soc. 

43.289.)  ,:;. 

Bismuth  ^'chloride,  Bi2Cl4. 

Very  deliquescent.  Decomp.  by  H2O,  dil. 
acids,  or  cone.  NH4Cl+Aq.  (Weber,  Pogg. 
107.  596.) 

Bismuth  trichloride,  BiCl3. 

Deliquescent.  Decomp.  by  H2O.  Sol.  in 
dil.  HCl+Aq,  and  alcohol.  Not  decomp.  by 
H2O  in  presence  of  citrates.  (Spiller.) 


0.08  g.  sol.  in  100  ccm.  liquid  H2S.  (An- 
tony, C.  C.  1905,  I.  1692.) 

Moderately  sol.  in  liquid  NH3.  (Gore,  Am. 
Ch.  J.  1898,  20.  827.) 

1  g.  Bids  is  sol.  in  5.59  g.  acetone  at  18°. 
Sp.  gr.  of  sat.  solution  18°/4°  =  0.9194.  (Nau- 
mann,  B.  1904,  37.  4331.) 

Sol.  in  acetone  and  in  methylal.  (Eidmann, 
C.  C.  1899,  II.  1014.) 

Sol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1369.) 

Sol.  in  ethyl  acetate.  (Naumann,  B.  1910. 
43.  314.) 

1  pt.  is  sol.  in  60.36  pts.  ethyl  acetate  at 
18°.  Sp.  gr  at  18°/40°  =  0.9106.  (Naumann, 
B.  1910,  43.  320.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Bismuth  chloride,  Bi3Cl8  (?). 

Decomp.  by  H2O.     (Dehe*rain,  C.  R.  54. 

724.) 

Bismuth  hydrogen  chloride,  2BiCl3,  HC1+ 
3H2O. 

Not  deliquescent.  Decomp.  by  H2O. 
(Engel,  C.  R.  106.  1797.) 

Bids,  2HC1.  (Jacquelain,  A.  ch.  (2)  62. 
363.) 

Bismuth  caesium  chloride,  BiCl3,  3CsCl. 

Decomp.  by  H2O.  SI.  sol.  in  cold  dil.  HC1+ 
Aq,  but  easily  sol.  on  warming.  (Brigham, 
Am.  Ch.  J.  14.  181.) 

2BiCl3,  3CsCl.    As  above.    (Brigham.) 

BiCl3,  6CsCl.  Easily  sol.  in  H2O  and  dil. 
HCl+Aq.  (Godeffroy,  B.  8.  9.) 

Does  not  exist.    (Brigham.) 

Bismuth  hydrazine  chloride,  BiCl3, 

3N2H4HC1. 

Sol.  in  acids,  from  which  it  is  pptd.  by  H2O. 
(Ferratini,  C.  A.  1912.  1613.) 

Bismuth  nitrosyl  chloride,  BiCl3,  NOC1. 

Very  deliquescent.  Decomp.  by  H2O. 
(Sudborough,  Chem.  Soc.  50.  662.) 

Bismuth  potassium  chloride,  BiCl3,  KC1+ 
H20. 

Decomp.  by  H2O.  Cannot  be  recryst.  ex- 
cept from  cone.  BiCl3+HCl.  Decomp.  by 
HCl+Aq  into  BiCl3,  2KC1+2H2O.  (Brig- 
ham,  Am.  Ch.  J.  14.  167.) 

BiCl3,  2KC1.  Decomp.  by  H2O.  (Arppe, 
Pogg.  64.  37.) 

Deliquescent. 

Sol.  in  H2O  with  decomp.  into  the  oxy- 
chloride  when  excess  H2O  is  used.  (Aloy, 
Bull.  Soc.  1906,  (3)  35.  397.) 

+2H2O.  Decomp.  by  H2O.  (Jacquelain, 
J.  pr.  14.  1.) 

Sol.  in  moderately  cone.  HCl+Aq. 

BiCl3,  3KC1.    Decomp.  by  H2O.    (Arppe.) 

Does  not  exist.    (Brigham.) 


92 


BISMUTH  RUBIDIUM  CHLORIDE 


Bismuth  rubidium  chloride,  BiCl3,  RbCl+ 
H20. 
Decomp.  by  H2O;  sol.  in  dil.  HCl+Aq, 
from  which  BiCl3,  3RbCl  crystallizes.    (Brig- 
ham,  Am.  Ch.  J.  14.  174.) 
BiCl3,  SRbCl.    Decomp.  by  H2O  ;  sol.  in  dil. 
HCl+Aq  without  decomp.     (Brigham.) 
BiCl3,  6RbCl.     Decomp.  by  H2O*;  sol.  in 
HCl+Aq  (Godeffroy,  B.  8.  9);  does  not  exist. 
(Brigham.) 
lOBiCls,  23RbCl  (?).     As  above.     (Brig- 
ham.) 

Bismuth   sodium  chloride,   BiCl3,   2NaCl+ 
H20. 
+3H2O.    Decomp.  by  H2O.    (Arppe,  Pogg. 
64.  237.) 
BiCl3,  SNaCl. 

Bismuth  thallous  chloride,  BiCl3,  3T1C1. 
Ppt.     (Ephraim,  Z.  anorg.  1909,  61.  254.) 
BiCl3,  6T1C1.    Ppt.    (Ephraim.)  . 

Bismuth  chloride  ammonia,  2BiCl3,  NH3. 
Stable.    (Dene-rain,  C.  R.  64.  724.) 
BiCl,,  2NH3.    (D.) 
BiCl3,  3NH3.    (D.) 

Bismuth  chloride  nitric  oxide,  BiCl3,  NO. 
Very  hygroscopic.     (Thomas,  C.  R.  1895, 
121.  129.) 

Solubility  of  freshly  pptd.  Bi(OH)3  in 
NaOH+Aq. 

g.  NaOH  per  1. 

g.  Bi  dissolved 
per  1.  at  20° 

g.  Bi  dissolved 
per  1.  at  100° 

400 
320 
240 
200 
160 
120 
80 
40 
20 

0.16 

0.11 
0.11 
0.10 
0.08 
0.07 
0.04 
trace 
0 

1.70 
1.20 

0.5 
0.5 

6^35 
0.2 
0.15 

(Moser,  Z.  anorg.  1909,  61.  386.) 

Solubility  of  freshly  pptd.  Bi(OH)3  in 
KOH+Aq. 

KOH  per  1.  g. 

g.  Bi  dissolved 
per  1.  at  20° 

g.  Bi  dissolved 
per  1.  at  100° 

560 
448 
336 
280 
224 
168 
112 
56 
28 

0.14 
0.11 
0.11 
0.10 
0.08 
0.06 
0.03 
•  trace 
0 

1.65 

1.20 

0'.5 
0.5 

o!3' 
0.2 
0.15 

(Moser,  Z.  anorg.  1909,  61.  386.) 

Bismuth  chloride  nitrogen  peroxide,  BiCl3, 
N02. 

Decomp.  by  moist  air,  but  stable  in  dry  air. 
(Thomas,  C.  R.  1896,  122.  612.) 

Bismuth  chloride  selenide. 
See  Bismuth  selenochloride. 

Bismuth  Zn'fluoride,  BiF3. 

Insol.  in  H20  or  alcohol.  (Gott  and  Muir, 
Chem.  Soc.  53.  138.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  827.) 

Bismuth  hydrogen  fluoride,  BiF3,  3HF. 

Deliquescent.  Decomp.  by  boiling  H20 
(Muir,  Chem.  Soc.  39.  21.) 

Bismuth  gold,  Au3Bi. 

Insol.  in  equal  pts.  of  HNO3  and  tartaric 
acids.  (Roessler,  Z.  anorg.  1895,  9.  71.) 

Bismuthous  hydroxide,  Bi(OH)3. 

Sol.  in  strong  acids.  Insol.  in  solutions  of 
alkalies,  alkali  carbonates,  (NH4)2CO3,  or 
NH4NO3;  or  of  amyl  amine  (Wurtz).  When 
recently  pptd.  is  sol.  in  NH4Cl+Aq,  but 
insol.  in  NH4NO3+Aq  (Brett,  1837).  Not 
'pptd.  in  presence  of  Na  citrates  (Spiller). 


Bi2O3,  2H20. 

Bi2O3,  H2O.    (Muir,  Chem.  Soc.  32.  131.) 

See  also  Bismuth  Znoxide. 


;,  Bi2O4,  H2O. 
Bi2O4,  2H2O.    (Wernicke,  Pogg.  141.  109.) 

Bismuthic  hydroxide  (Bismuthic  acid),  Bi2O5, 
H2O. 

Insol.  in  H2O;  easily  decomp.  by  acids. 
(Fremy,  A.  ch.  (3)  12.  495.)  Decomp.  by 
H2SO4;  not  attacked  by  SO2+Aq;  neither 
dissolved  nor  decomp.  by  dil.  HNO3+Aq,  but 
slowly  converted  into  an  allotropic  modifica- 
tion (?).  Partially  decomp.  by  cone.  HNO3. 
Slowly  but  wholly  dissolved  by  hot  cone. 
BNO3.  SI.  sol.  in  cone.  KOH+Aq.  (Arppe.) 

Sol.  in  about  100  pts.  boiling  KOH+Aq,  so 
cone,  that  it  solidifies  on  removing  the  lamp 
'Muir,  Chem.  Soc.  51.  77.) 
1  Bi-jO,,,  2H2O.    (Bodeker,  A.  123.  61.) 

Does  not  exist.    (Hoffmann  and  Geuther.) 

Bismuth  iodide,  BiI3. 

Not  attacked  by  cold  H2O,  but  by  boiling, 
BiOI  is  formed.  100  pts.  absolute  alcohol 
dissolve  3^  pts.  salt  at  20°.  (Gott  and  Muir, 
~!hem.  Soc.  57.  138.) 

Sol.  in  HNO3,  and  HI+Aq,  from  which  it 
TT  O  or  alcohol.    S(-  '    ~ 
(Rammelsberg.) 


3,  q,   rom  wc 

s  repptd.  by  H2O  or  alcohol.    Sol.  in  KI+Aq 
or  KOH+Aq. 


BISMUTH  OXIDE 


93 


SI.  sol.  in  liquid  NH3.    (Franklin,  Am.  Ch. 

Bismuth  Zn'oxide,  Bi2O3. 

J.  1898,  20.  827.) 
100  g.  absolute  alcohol  dissolve  3.5  g.  BiI3 
at  20°.    (Gott  and  Muir,  Chem.  Soc.  57.  138.) 

Insol.  in  H2O.    Sol.  in  cone,  acids. 
Solubility  of  Bi2O3  in  HNO3+Aq  at  20°. 

Sol.  in  acetone.     (Naumann,  B.  1904,  37. 

In  100  g.  of  the 

4328.) 

liquid  p! 

100  pts.  methylene  iodide  dissolve  0.15  pt. 
BiI3  at  12°,  and  very  little  more  at  higher 

Solid  phase 

g.  Bi203 

g.  N205 

temperatures.    (Retgers,  Z.  anorg.  3.  343.) 
Sol.   in   methyl  acetate.      (Naumann,   B. 

0.321 
0.337 

0.963 
0  Q82 

Bi2O3.N2O5.2H2O 

u 

1909,  42.  3790.) 

3^54 

\J  .  t/O^ 

4.68 

(I 

Bismuth  hydrogen  iodide,  BiI3,  HI+4H2O. 

6.37 
13.67 

7.17 
12.50 

a 
« 

(Arppe,  Pogg.  44.  248.) 

14.85 

13.31 

II 

18.74 

15.90 

Bi2O3.N2O5.H2O 

Bismuth  caesium  iodide,  3CsI,2BiI3. 

23.50 

19.21 

a 

Very  si.  sol.  in  H2O.     (Wells,  Am.  J.  Sci. 

23.50 

19.29 

(( 

1897,  (4)  3.  464.) 

27.15 

20.96 

ei 

28.11 

21  .  64 

« 

Bismuth  calcium  iodide,  2BiI3,  CaI2  +  18H2O. 

29.50 

22.53 

a 

Deliquescent;  decomp.  by  H2O.     (Linau, 

30.19 

22.90 

(1 

Pogg.  111.  240.) 

31.48  . 

23.70 

a 

32.93 

24.83 

|Bi2O3.N2O5.H2O+ 

Bismuth  magnesium  iodide,  2BiI3,  MgI2  + 

32.80 

24.86 

{Bi203.3N206.10H20. 

12H2O. 

32.67 

24.70 

Bi2O3.3N2O5.10H2O. 

Deliquescent;  decomp.  by  H2O.     (Linau, 

32.59 

24.60 

a 

Pogg.  111.  240.) 

32.24 

24.68 

(i 

30.74 

25.13 

u 

Bismuth  potassium  iodide,  BiI3,  4KI. 

29.83 

25.30 

(( 

Ppt.    (Arppe,  Pogg.  44.  237.) 

24.16 

28.25 

n 

BiI3,  SKI.    (Astre,  C.  R.  110.  1137.) 

16.62 

35.40 

(i 

BiI3,  2KI.    Sol.  in  acetic  ether.    (Astre.) 

12.17 

43.37 

( 

+4H2O.    Sol.  in  small  amt.  H2O  without 

11.66 

46.62 

i 

pptn.,  but  decomp.  by  much  H2O. 

11.19 

49.38 

t 

BiI3,  2KI,  HI.    (Arppe.) 

11.19 

50.20 

t 

2BiI3,  3KI+2H2O.    (Astre.) 
BiI3,KI+H2O.  Decomp.  by  H2O.  (Nickles, 
C.  R.  61.  1097.) 
2BiI3,  KI.    Sol.  in  acetic  ether.    (Astre.) 

15.20 
20.76 

27.85 

54.66 
53.75 

51.02 

i 

(Bi2O3.3N2O5.10H2O+ 
Bi2O3.3N2O5.3H2O.     , 

8.58 

68.28 

Bi2O3.3N2O5.3H2O. 

Bismuth  sodium  iodide,  BiI3,  NaI+H2Q. 

4.05 

74.90 

a 

Deliquescent;  decomp.  by  H2O.     (Nickles, 

(Rutten,  Z.  anorg.  1902,  30.  386.) 

C.  R.  51.  1097.) 

2BiI3,  3NaI  +  12H2O.    As  above.     (Linau, 

T*                    -I  4  H        O  A  f\    \ 

Solubility  of  Bi2O3  in  HNO3+Aq  at  t°. 

Pogg.  111.  240.) 

t° 

%Bi2Os 

%N2O5 

Solid  phase 

Bismuth  zinc  iodide,  2BiI3,  ZnI2+12H2O. 
Very  deliquescent.   (Linau,  Pogg.  111.  240.) 

IF 

20.8 
24.02 

17.1 
19.1 

Bi2O3.N2O5.H2O 

n 

Bismuth  iodide  ammonia,  BiI3,  3NH3. 

31.09 
31.2 

23.8 
23.9 

jBi203.N2O5.H2O+ 
jBi2O3.3N2O5.10H2O 

Decomp.  by  H2O.    (Rammelsberg.) 

30° 

34.2 

26.5 

ii 

Bismuth  iodide  zinc  bromide. 

28.2 

29.6 

Bi2O3.3N2O5.10H2O 

Sol.  in  H2O.    (Linau,  Pogg.  111.  240.) 

16.1 

47.7 

u 

Bismuth  nitride. 

65° 

5.55 

7.44 

Bi2O3.N205.H2O 

Explosive.    (Fischer,  B.  1910,  43.  1471.) 
BiN.    Ppt.  '  Decomp.  by  H2O  or  dil.  acids. 

27.62 
40.80 

22.46 
31.60 

u 

Bi2O3.  N2O5  .  H2O+Bi2O3. 

(Franklin,  J.  Am.  Chem.  Soc.  1905,  27.  847.) 

3N2O5.10H2O 

37.82 

35.80 

Bi2O3.3N2O5.10H2O 

Bismuth  dioxide,  Bi202. 

QK     7<3 

A  *7     AO 

(Bi2O3.3N2O5.10H2O  + 

Sol.   in   cone.   HNO3+Aq.     Decomp.   by 

OO  .  4  O 

4/  .  UJ 

|Bi2O3.3N2O5.3H2O 

strong  acids,  and  boiling  KOH+Aq. 

4.59 

77.90 

Bi2O3.3N2O5.3H2O 

Decomp.   by   H2O.      (Tanatar,   Z-.   anorg. 

1901,  27.  438.) 

(Rutten.) 

94 


BISMUTH  OXIDE 


Solubility  of  Bi2O3  in  HNO3+Aq  at  t°. 

Bismuth  phosphide,  BiP. 

(Cavazzi.) 

Bismuth  /nselenide,  Bi2Se3. 
Insol.  in  H2O,  alkalies,  or  alkali  sulphides 
+Aq;  si.  attacked  by  HCl+Aq;  oxidized  by 
HNO3+Aq.    (Schneider,  Pogg.  94.  628.) 
Min.  Frenzelite. 

Bismuth  potassium  selem'de. 
See  Selenobismuthite,  potassium. 

Bismuth  selenochloride,  BiSeCl. 
Not  attacked  by  H2O;  very  si.  sol.  in  HC1+ 
Aq;  easily  and  completely  sol.  with  decomp. 
in  HNO3+Aq.    (Schneider.) 

Bismuth  ^sulphide,  Bi2S2+2H2O  (?). 
Insol.  in  H2O.    Decomp.  by  HCl+Aq. 

Bismuth  Znsulphide,  Bi2S3. 
Insol.  in  H2O. 
1  1.  H2O  dissolves  0.35  x  ICh8  moles  Bi2S3 
at  18°.    (Weigel,  Z.  phys.  Ch.  1907,  58.  294.) 
Easily  sol.  in  moderately  dil.  HNO3+Aq, 
and  cone.  HCl+Aq,  with  separation  of  S. 
Insol.  in  alkalies,  alkali  sulphides,  Na2S2O3, 
or  KCN+Aq;  insol.  in  NH4C1,  or  NH4NO3  + 
Aq  (Brett).    Insol.  in  potassium  thiocarbon- 
ate+Aq.    (Rosenbladt,  Z.  anal.  26.  15.) 
Insol.  in  alkali  hydroxides  or  alkali  hydro- 
sulphides. 
Insol.  in  2N-(NH4)2S+Aq. 
0.0090  g.  Bi2S3  is  sol.  in  100  cc.  N-Na2S2+ 
Aq  at  25°.     (Knox,  Chem.  Soc.   1909,   95. 
1764.) 
Somewhat  sol.  in  Na2S+Aq.     75  cc.   of 
Na2S+Aq  (sp.  gr.  1.06)  dissolve  an  amt.  of 
Bi2S3  corresponding  to  0.031  g.  Bi2O3.    (Still- 
man,  J.  Am.  Chem.  Soc.  1896,  18.  683.) 

t° 

%Bi2Os 

%N2O6                  Solid  phase 

72° 
75° 
80° 

37.23 
36.74 
39.75 

47.76 
47.91 
45.16 

Bi2O3.3N2O5.4H2O 

(( 

u 

9° 
20° 
30° 
50° 
64° 
65° 
75.5° 
,72° 

31.2 
32.8 
34.2 
36.9 
40.6 
40.8 
45.4 
45.9 

23.9 
24.8 
26.4 
28.9 
31.1 
31.6 
34.6 
35.6 

Bi2O3.3N205.10H2O  + 
Bi2O3.N205.H2O 

11.5° 

20° 
50° 
65° 

25.36 

27.85 
32.22 
35.73 

52.57 

51.02 
49.29 
47.02 

}    Bi2Os.3N2O5.10H2O  + 

J      Bi2O3.3N2O5.3H2O 
(i 

c( 
n 

(Rutten.) 
Solubility  in  NaOH+Aq  at  25°. 

Cone,  of  NaOH         g.  Bi2Os  in  100  cc.  of  solution. 
Mol/l.                                   Mean  result. 

1.0                       0.0013^0.0002 
2.0                       0.0026^0.0002 
3.0                       0.0049±0.0005 

(Knox,  Chem.  Soc.  1909,  95.  1767.) 

Insol.  in  acetone.     (Eidmann,  C.  C.  1899, 
II.  1014.) 
Min.  Bismite.    Easily  sol.  in  HNO3+Aq. 
See  also  Bismuthous  hydroxide. 

Sol.  in  cone.  HCl+Aq,  with  evolution  of 
Cl;  in  oxygen  acids  with  evolution  of  O.  Less 
easily  sol.  in  cone.  H2SO4  than  in  HNO3,  or 
HCl+Aq. 

Bismuth  oxide,  Bi4O9  (?). 
(Hoffmann  and  Geuther.) 

Bismuth  peroxide,  Bi2O6. 

Sol.  in  dil.  acids.  Combines  with  H2O  to 
form  bismuthic  hydroxide,  which  see.  (Hase- 
broek,  B.  20.  213.) 

Bismuth  oxybromide,  etc. 
See  Bismuthyl  bromide,  etc. 

Bismuth  palladium,  PdBi2. 

Insol.  in  equal  pts.  HNO3  and  tartaric  acids 
(Roessler,  Z.  anorg.  1895,  9.  70.) 

Bismuth  platinum,  PtBi2. 

Insol.  equal  pts.  HNO3  and  tartaric  acids 
(Roessler,  Z.  anorg.  1895,  9.  69.) 


Solubility  in  Na2S+NaOH+Aq  at  25°. 


Cone,  of  Na2S 
Mol/l 

Cone,  of  NaOH 
Mol./l. 

g.  Bi2Ss  in  100  cc. 
of  solution 

0.5 
1.0 

1.0 
1.0 

0.0185 
0.0838 

(Knox,  Chem.  Soc.  1909,  95.  1763.) 

Bismuth  sulphide  pptd.  from  acid  solution 
is  not  dissolved  by  subsequent  treatment  with 
K2S+Aq.  (Stone,  J.  Am.  Chem.  Soc.  1896, 
18.  1091.) 

Sol.  in  K2S+Aq.  (Ditte,  C.  R.  1895,  120. 
187.) 

Solubility  in  K2S+KOH+Aq  at  25°. 


Cone,  of  K2S 
Mol./l. 

Cone,  of  KOH 
Mol./l. 

g.  Bi2S3  in  100  cc. 
of  solution 

0.5 
1.0 

1.25 

1.0 
1.0 
1.25 

0.0240 
0.1230 
0.2354 

(Knox,  Chem.  Soc.  1909,  95.  1763.) 

BISMUTHYL  FLUORIDE 


95 


Solubility  in  alkali  sulphides +Aq  at  25C 


Alkali 
sulphide 

Cone,  of  alkali 
sulphide  Mol.  /I. 

g.  BizSs  in  100  cc. 
of  solution 

Na2S 

0.5 
1.0 
1.5 

0.0040 
0.0238 
0.1023 

K2S 

0.5 
1.0 
1.25 

0.0042 
0.0337 
0.0639 

(Knox,  Chem.  Soc.  1909,  95.  1762.) 

Decomp.  by  FeCl3+Aq.  (Cammerer,  C.  C. 
1891,  II.  525.) 

Insol.  in  KCN+Aq.  (Hoffmann,  A.  1884, 
223.  134.) 

Min.  Bismuthiniie.  Easily  sol.  in  HNO3+ 
Aq. 

Bismuth  cuprous  sulphide,  Bi2S3,  Cu2S. 

Insol.  in  H2O.  Sol.  with  decomp.  in  HNO3 
+Aq.  (Schneider,  J.  pr.  (2)  40.  564.) 

Min.  Emplectonite. 

Bismuth  potassium  sulphide,  Bi2S3,  K2S. 

(Schneider,  Pogg.  136.  460.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

Bi2S3,4K2S+4H2O.  Decomp.  by  H2O. 
Very  sol.  in  K2S-j-Aq.  Efflorescent  in  dry 
air.  (Ditte,  C.  R.  1895,  120.  186.) 

See  also  Sulphobismuthite,  potassium. 

Bismuth  silver  sulphide,  Bi2S3,  Ag2S. 

Insol.  in  cold  HC1,  or  HNO3.  Sol.  in  warm 
HNO3  with  separation  of  S,  in  boiling  HC1 
with  separation  of  H2S. 

Min.  Plenargyrite,  Matildite. 

(Schneider,  J.  pr.  1890,  (2)  41.  414.) 

Bismuth  sodium  sulphide,  Bi2S3,  Na2S. 
(Schneider.) 

Bismuth  sulphide  telluride,  Bi2S3,  2Bi2Te3. 

Min.  Tetradymite.  Sol.  in  HNO3  with  sepa- 
ration of  S. 

Bi2S2,  2Bi2Te. 

Min.  Joseite.    As  above. 

Bismuth  sulphobromide,  BiSBr2. 

(Muir  and  Eagles,  Chem.  Soc.  1895,  67.  91.) 

Bismuth  sulohochloride,  BiSCl. 

Insol.  in  H2O  or  dil.  HCl-j-Aq.  Sol.  in 
cone.  HC1,  or  HNO3+Aq.  Decomp.  by 
alkalies +Aq.  (Schneider,  Pogg.  93.  464.)  , 

Bismuth  sulphoiodide,  BiSI. 

Not  attacked  by  boiling  H2O,  and  dil.  acids. 
Decomp.  by  hot  cone.  HCl+Aq,  and  HNO3+ 
Aq.  KOH+Aq  dissolves  out  I2.  (Schneider, 
Pogg.  110.  114.) 


Bismuth  telluride,  Bi2Te3. 

Min.  Tetradymite.    Sol.  in  HNO3+Aq. 
See  also  Bismuth  sulphide  telluride. 

Bismuthic  acid,  HBiOs. 
See  Bismuthic  hydroxide. 

Potassium  bismuthate,  KBi03. 

Sol.  in  H2O.    (Arppe.) 

KH(BiO3)2.    Insol.  in  H2O. 

Not  decomp.  by  boiling  H20.  (Andre,  C. 
R.  113.  860.) 

No  salts  of  HBiO3  can  exist.  (Muir  and 
Carnegie,  Chem.  Soc.  51.  77.) 

Bismuthicotungstic  acid. 

Ammonium  bismuthicotungstate,  3(NH4)2O, 

2Bi2O3,  11WO3+10H2O. 
A  yellow  oil  which  dries  to  a  yellow  glass. 
(E.  F.  Smith,  J.  Am.  Chem.  Soc.  1903,  25. 
1232.) 

Potassium  bismuthicotungstate,  3K2O, 

2Bi203,l  1WO3  +  15H2O. 
A  yellow  oil  which  dried  to  a  pale  yellow 
glass.     (E.  F.  Smith,  J.  Am.  Chem.  Soc.  1903, 
26.  1233.) 

Strontium  bismuthicotungstate,  3SrO, 

2Bi2O3,llWO3+llH2O. 
A  yellow  wax,  insol.  in  pure  H2O,  but  sol. 
in  H2O  containing  a  few  drops  HNO3.     (E. 
F.  Smith,  J.  Am.  Chem.  Soc.  1903,  25. 1233.) 

Bismuthyl  bromide,  BiOBr. 

Insol.  in  H2O;  sol.  in  moderately  cone. 
HBr+Aq. 

Insol.  in  H20.  (Herz,  Z.  anorg.  1903,  36. 
348.) 

Bi8O9Br6.  Insol.  in  H2O;  easily  sol.  in 
cone.  HC1,  or  HNO3+Aq;  less  sol.  in  dil. 
HNO3+Aq. 

BiuOi3Br7.  As  the  preceding  comp. 
(Muir.) 

Bismuthyl  chloride,  BiOCl. 

Insol.  in  H2O  or  dil.  acids.  Sol.  in  cone. 
HC1,  orHNO3+Aq. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch.  J. 
1898,  20.  827.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

+H2O.    (Heintz,  Pogg.  63.  55.) 

+3H2O.     (Phillips,  Br.  Arch.  (1)  39.  41.) 

Bi7O9Cl3.    (Arppe.) 

Bi02Cl3.  Insol.  in  H2O;  sol.  in  hot  HC1,  or 
HNO3+Aq.  (Muir.) 

Bismuthyl  fluoride,  BiOF. 

Insol.  in  H2O;  sol.  in  HC1,  HBr,  or  HI-f-Aq. 
(Gott  and  Muir,  Chem.  Soc.  33.  139.) 

BiOF,  2HF.    Insol.  in  H2O. 


96 


BISMUTHYL  IODIDE 


Bisinuthyl  iodide,  BiOI. 

Not  decomp.  by  HsO  or  alkaline  solutions 
Sol.  in  HCl+Aq.  Decomp.  by  HNO3+Aq 
(Schneider,  J.  pr.  79.  424.) 

Insol.  in  KC1,  or  KI+Aq. 

3BiOI,7Bi2O3.  Sol.  in  dil.  HC1;  decomp 
by  HNO3;  insol.  in  boiling  H20  and  alkali 
(Blyth,  C.  N.  1896,  74.  200.) 

BiI3,  5Bi2O3.  Ppt.  SI.  sol.  in  HC2H3O2+ 
Aq.  Not  decomp.  by  H2O.  (Fletcher  anc 
Cooper,  Pharm.  J.  (3)  13.  254.) 

4BiI3,  5Bi2O3.  Easily  sol.  in  HCl+Aq 
Decomp.  by  HNO3+Aq.  SI.  attacked  by 
H2SO4;  somewhat  sol.  in  H2C4H4O6,  anc 
KHC4H4O6+Aq. 

Sol.  in  (NH4)2S,  and  KOH+Aq.  (Storer's 
Diet.) 

Bisinuthyl  sulphide,  Bi6O3S. 

(Hermann,  J.  pr.  76.  452.) 

Bi2O3S.  Insol.  in  H2O.  (Scherpenberg, 
C.  C.  1889,  II.  641.) 

Bi403S. 

Min.  Karelinite. 

Boracic  acid. 
See  Boric  acid. 

Borax. 

See  TeZraborate,  sodium. 


Or,  sat.  aqueous  solution  contains  at — 

19°  3.75%H3BO3. 

25°      6.27  " 

37.5°    7.32  ' 

50°      8.96  ' 

62.5°    14.04  ' 

75°     17.44  ' 

87.5°        21.95   ' 
100°  25.17  < 

(Brandes  and  Firnhaber,  Arch.  Pharm.  7.  50.) 
1  litre  H2O  dissolves  at — 


0° 
12° 
20° 
40° 
62° 
80° 
102^ 


19.47g.  H3BO3. 

29.20  " 

39.92" 

69.91" 
114.16" 
168.15" 
291.16" 


(Ditte,  C.  R.  85.  1069.) 

1 1.  H2O  dissolves  0.901  mol.  H3BO3  at  25°. 
(Herz,  Z.  anorg.  1910,  66.  359.) 

1 1.  H20  dissolves  0.898  mol.  H3BO3  at  25°. 
Sp.  gr.  of  the  solution  =  1.0 168.  (Miiller,  Z. 
phys.  Ch.  1907,  67.  529.) 

1 1.  H2O  dissolves  0.887  mol.  H3BO3  at  25° 
and  1.025  mol.  at  30°.  (Ageno  and  Valla, 
1st.  Ven.  (VIII)  14.  II,  331.) 

Solubility  in  H2O  at  t°. 


Boric  acid,  anhydrous,  B20a. 

t° 

g.  HsBOs  in  100  g.  of  the  solution 

See  Boron  Znoxide. 

0 

2.59 

Metabolic  acid,  HB02. 

12.2 
21 

3.69 
4.90 

Sol.  in  H2O. 

31 

6*44 

SI.  sol.  in  hot  glacial  acetic  acid.     (Holt, 

40 

8.02 

Chem.  Soc.  1911,  100.  (2)  720.) 

50 

10.35 

60 

12.90 

Orthobonc  acid,  H3B03. 

69.5 

15^58 

Sol.  in  33  pts.  H2O  at  10°. 

80 

19.11 

25          "         "  20°. 
"          3         "         "  100° 

90 

23.30 

(Berzelius.) 

99.5 
108 

28.10 
36.7 

Sol.  in  20  pts:  H2O  at  18.75°.    (Abl.) 
100  pts.  HsO  at  100°  dissolve  2  pts.    (Ure's  Diet.) 

115 
120 

45.0 
52.4 

1  pt.  crystallized  acid  dissolves  in  — 
25.  66  pts.  H20  at  19°. 
14.88                 "     25°. 

(Nasini  and  Ageno,  Z.  phys.  Ch.  1909,  69. 

483.)    ' 

12.66                 "     37.5°. 

Solubility   curve   for   orthoboric    acid    in 

10.16                 "     50°. 
6.12                 "     62.5°. 
4  73                 "     75° 

I2O  at  various  temp,  up  to  120°.     (Nasini 
and  Ageno,  Gazz.  ch.  it.  1911,  41.  (1)  131. 

3.55                 "     87.5°. 

Sp.  gr.  of  H3BOs  +Aq  sat.  at  8°  =  1.014.     (Anthon,  A  . 
•4.  241.) 

2.97                 "  100°. 

Sp.  gr.  of  H3BO3+Aq  sat.  at  15°  =  1.024S.    (Stolba.  J. 

Or,  100  pts.  H2O  dissolve  at— 

pr.  90.  457.) 

19°              3.  9  pts.  H3BO3. 

oc°                   «   o    «               i 

Sp.  gr.  of  H3B03+Aq  at  15°. 

Zo                    O.o 

37.5°          7.8   " 

'%H3BO3 

Sp.  gr.         %H3B03 

Sp.  gr. 

50°              9.8   "            ' 
62.5°         16.0   " 
75°            21.0   " 

1 

2 

Q 

1.0034           4 
1.0069      Sat.  sol. 

1.0147 
1.015 

87.5°        28.0   " 

O 

1  .  U1UO              .  .  . 

100°            34.0   "           ' 

(Gerlach,  Z.  anal.  28.  473.) 

BORIC  ACID 


97 


Sp.  gr.  of  H3BO3+Aq  at  18°. 
%H3BO3    0.776       1.92        2.88        3  612 
Sp.gr.         1-0029     1.0073     1.0109     1.013 
(Bock,  W.  Ann.  1887,  30.  638.) 

Volatile  with  steam. 
More  sol.  in  dil.  HCl+Aq  than  in  H2O 
Sol.  in  warm  cone.  H2SO4,  HC1,  or  HNO3  + 
Aq. 

Solubility  in  HCl+Aq  at  25°. 

Solubility  in  KOH+Aq. 
See  Berates,  potassium. 
Solubility  in  NaOH+Aq. 
See  Borates,  sodium. 

Solubility  in  LiCl+Aq  at  25°. 

Millimols  LiCI  in 
10  ccm.  of  the  solution 

Millimols  HaBOs  in  10  ccm. 
of  the  sat.  solution 

7'l 
10.3 
22.3 
37.2 

9.01 
8.13 
7.65 
6.42 
5.02 

Millimols  HC1  in           1 
10  ccm.  of  the  solution 

Vlillimois  H3BO3  in  10  ccm 
of  the  sat.  solution 

7.'6 
13.7 

9.01 
7.69 
6.66 

(Herz,  Z.  anorg.  1910,  66.  359.) 
Solubility  in  KCl+Aq  at  25°. 

(Herz,  Z.  anorg.  1910,  66.  359.) 
Solubility  of  H3BO3  in  HCl+Aq  at  16°. 

Millimols  KC1  in 
10  ccm.  of  the  solution 

Millimols  HaBOj  in  10  ccm. 
of  the  sat.  solution 

Normality  of  HC1 

Normality  of  HsBOa 

"l.9 

7.9 
15.6 
30.6 

9.01 
9.20 
9.44 
9.80 
10.75 

0. 
0.130 
0.260 
0.390- 
1.30 
2.16 
4.32 
6.00 
7.08 
8.74 
9.51 

0.907 
0.895 
0.870 
0.842 
0.645 
0.542 
0.308 
0.338 
0.327 
0.327 
0.338 

(Herz.) 
Solubility  in  RbCl+Aq  at  25°. 

Millimols  RbCl  in 
10  ccm.  of  the  solution 

Millimols  HsBOa  in  10  ccm. 
of  the  sat.  solution 

ii'6 

25.3 

9.01 
9.66 
10.60 

(Herz,  Z.  anorg.  1902,  33.  354.) 
Solubility  in  HF+Aa  at  26°. 

(Herz.) 
Solubility  in  NaCl+Aq  at  25°. 

(1)                       <2> 
Titerof           Titer  after 
wp          saturation  wit 
H3B03  at  26° 

(3) 
Titer  after         f%\    /2) 
addition        equals  free 

h   mannitol        b°ric  add 

Millimols  NaCl  in 
10  ccm.  of  the  solution 

Millimols  H3BO3  in  10  ccm. 
of  the  sat.  solution 

3.21n.      1.61 
2.80n.      1.25(1.40?) 

2.36      0.75 
2.21      0.96(0.81?) 

'8.'2 
15.2 
29.4 

9.01 
8.49 

8.25 
8.20 

The  values  0.75  and  0.81   represent  the 

fluorboric  acid  resulting  from   the  original 
concentration  of  HF+Aq. 

(Abegg,  Z.  anorg.  1903,  35.  145.) 

Solubility  of  H3BO3  in  acids +Aq  at  26°. 


Acid 

Normality  of 
the  acid 

Normality  of  HsBOs 

H2S04 

0.548 

2.74 
5.48 
8.75 

0.746 
0.518 
0.312 
0.092 

HNO3 

0.241 
1.206 
1.607 
2.411 
5.96 
7.38 

0.818 
0.676 
0.593 
0.567 
0.268 
0.238 

(Herz,  Z.  anorg.  1903,  34.  205.) 

(Herz.) 

Solubility  in  H2O  is  increased  by  presence 
of  KC1,  KNO3,  K2SO4,  NaNOa  and  Na2SO4. 

In  general  the  solubility  in  H2O  is  increased 
>y  the  presence  of  both  electrolytes  and  non- 
electrolytes.  (Bogdan,  C.  C.  1903,  II.  2.) 

Sol.  in  borax +Aq.  (McLauchlan,  Z.  anorg. 
903  37  371  ) 

SI.'  soL  in  liquid  NH3.  (Franklin,  Am.  Ch. 
r.  1898,  20.  827.) 

Unattacked  and  undissolved  by  liquid  N02. 
Frankland,  Chem.  Soc.  1901,  79.  1362.) 

Sol.  in  6  pts.  alcohol  (Wittstein),  5  pts. 
soiling  alcohol  (Wenzel).  Only  traces  .dis- 
olve  in  anhydrous  ether.  (Schiff.)  Sol.  in 
00  pts.  ether.  (Hager's  Comm.)  Sol.  m 
everal  essential  oils. 

1  1.  H2O  sat.  with  amyl  alcohol  dissolves 
1.8952  mol.  H3BO3  at  25°.  (Auerbach,  Z. 
Jiorg.  1903,  37.  357.) 


98                                                            BORIC  ACID 

Solubility  of  H3BO3  in  amyl  alcohol  -{-Aq  at  t°. 

Sp.  gr.  of  amyl  alcohol+Aq  sat.  with  H3BO3. 

M  =millimols  H3BO3  in  1  1.  of  H2O. 
A  =  millimols  H3BO3  in  1  1.  of  alcohol. 

g.  water  in  1  1.  of  alcohol  + 
Aq 

d25°/4° 

t° 

M 

A 

32.481 

0.82229 

15° 

607.2 
589.3 

176.4 
177.4 

35.465 
37.339 
42.479 

0  .  82324 
0.82321 
0.82392 

. 

589.0 

177.1 

45  .  175 

0.82447 

• 

586.0 
427.4 
425.8 

173.4 
127.6 
127.0 

45.636 

47.883 
51.461 

0.82456 
0.82454 
0.82527 

289.1 
894.0 
372.0 
371.8 

84.9 
264.0 
110.0 
110.8 

52.043 
59.270 
63.179 
64.254 

0.82585 
0.82699 
0.82739 
0.82779 

25° 

301.2 

85.7 

66.403 
66.624 

0.82701 
0.82670 

180.8 
49.15 
51.04 
26.02 

54.0 
15.45 
15.45 
8.05 

68.253 
69.211       . 
75.610 

0.82856 
0.82884 
0.  82999  (?) 

(M  tiller.) 

35° 

146.3 

44.27 

(Mtiller,  Z.  phys.  Ch.  1907,  67.  514.) 


Solubility  of  H3BO3  in  amyl  alcohol  and  NaCl+Aq  at  25C 


Water  phase 


Amyl  alcohol  phase 


NaCl  normality 

mol.  HsBOs 

Sp.  gr.  25°/4° 

1  1.  contains 

mol.  H2O 

mol.  amyl  alcohol 

mol.  HaBOs 

0.00 

0.880 

0.8296 

4.10 

8.39 

0.2640 

0.945 

0.866 

0.8277 

3.55 

8.49 

0.2638 

1.490 

0.850 

0.8268 

3.27 

8.54 

0.2689 

1.865 

0.844 

0.8259 

3.03 

8.56 

0.2724 

2.355 

0.833 

0.8254 

2.86 

8.59 

0.2850 

2.845 

0.827 

0.8247 

2.62 

8.62 

0.2877 

3.06 

0.810 

0.8241 

2.39 

8.66 

0.2891 

3.48 

0.810 

0.8240 

2.32 

8.69 

0.3006 

3.57 

0.807 

0.8236 

2.15 

8.70 

0.3066 

4.01 

0.801 

0.8233       . 

1.99 

8.72 

0.3162 

4.28 

0.798 

0.8229 

1.78 

8.75 

0.3210 

(Miiller) 


Solubility  in  hydroxy-compounds+Aq  at  25°. 


Organic  substance 
added 

Mol.  of  organic  sub- 
stance in  100  mol.   of 
the  mixture 

Mol.  of  boric  acid  sol. 
in  1  1.  of  solution 

Sp.  gr.  of  the  pure 
mixture 

Sp.  gr.  of  the  mixture 
sat.  with  boric  acid 

Lactic  acid 

2.321 
6.819 
18.77 
36.33 

1.07 
1.61 

1.86 
2.08 

1.0252 
1.0722 
1  .  1405 
1.2023 

1.0444 
1.0986 
1  .  1635 
1.2254 

Glycerine 

24.64 
46.75 
67.71 

90.58 

1.208 
2.132 
2.96 

3.78 

1  .  1574 

1.2370 
1.2531 

1.1707 
1.2260 
1.2526 
1.2710 

BORIC  ACID 


Solubility  in  hydroxy-compounds,  etc. — Continued 


Organic  substance 
added 

Mol.  of  organic  sub- 
stance in  100  mol.  of 
the  mixture 

Mol.  of  boric  acid  sol. 
in  1  1.  of  solution 

Sp.  gr.  of  the  pure 
mixture 

Sp.  gr.  of  the  mixture 
sat.  with  boric  acid 

Mannitol 

0.790 
0.810 
0.945 
1.585 

1.007 
1.015 
1.029 
1.136 

l'0244 
1.0288 
1.0475 

1.0425 
1.0433 

Dulcitol 

0.065 
0.130 
0.260 

0.8876 
0.9078 
0.9360 

0.9995 
1.0018 
1.0060 

1.0686 
1.0212 
1.0260 

(Miiller.) 


Solubility  of  H3BO3  in  alcohols +Aq  at  25°. 
M  =Mol.  of  alcohol  in  100  mol.  of  alcohol+Aq. 
H3BO3  =  Mol.  of  H3BO3  in  1  1.  of  the  solution. 
d1=Sp.  gr.  of  alcohol+Aq. 
d2=Sp.  gr.  of  alcohol+Aq  sat.  with  H3BO3. 


Alcohol  added 

M 

HsBOs 

di 

da 

Methyl  alcohol 

11.74 

0.895 

28.64 

1.012 

36.02 

1.098 

43.95 

1.161 

52.31 

1.307 

100 

'    2.900 

0.7924 

0.8904 

Ethyl  alcohol 

8.996 

0.829 

22.28 

0.800 

44.46 

0.729 

55.62 

0.700 

79.89 

0.893 

88.10 

1.105 

99.26 

1.527 

0.7860 

0.8353 

n-Propyl  alcohol 

23.66 
53.63 

0.6437 
0.4569 

0.9043 
0.8231 

0.9193 
0.8570 

83.65 

0.5776 

0.8133 

0.8466 

100 

0.961 

0.8010 

0.8297 

i-Butyl  alcohol 

0.70 
2.15 

0.884 
0.857 

0.9923 
0.9853 

1.0124 
0.0038 

2.18 

0.857 

0.9855 

0.0046 

71.4 

0.323 

0.8173 

0.8351 

77.1 

0.347 

0.8133 

0.8220 

85  6 

0.4212 

0.8081 

0.8195 

100 

0.6927 

0.7984 

0.8172 

i-Amyl  alcohol 

0.448 
0.520 

0.883 
0.880 

0.9943 
0.9936 

1.0132 
1.0125 

0.5251 

0.880 

0.9931 

1.0123 

- 

67.  262 

0.2584 

0.8232 

0.829      . 

75.54 

0.2722 

0.8183 

0.8253 

83.40 

0.3190 

0.8142 

0.8223 

100 

0.5703 

0.8068 

0.8220 

i  Water  sat.  with  alcohol.                                                              2  Alcoh°l  sat"  Wlth  water' 

(Miiller.) 


100 


BORIC  ACID 


Easily  sol.  in  acetone.    (Krug  and  M'Elroy, 
J.  Anal.  Ch.  6.  184.) 

Solubility  in  acetone -}-Aq  at  20°. 
A  =  ccm.  acetone  in  100  ccm.  acetone-fAq. 
H3BO3  =  millimols  H3BO3  in  100  ccm.  of 
the  solution. 


A 


0 

20 
30 
40 
50 
60 
70 
80 
100 


HaBO» 


79.15 
81.71 
83.35 

82.74 
81.61 
76.40 
67.62 
55.05 
8.06 


(Herz,  Z.  anorg.  1904,  41.  319.) 

100  g.  pure  anhydrous  ether  dissolve  0.00775 

g.  H3B03. 
100  g.  ether  sat.  with  H»O  dissolve  0.2391  g. 

H3BO3. 

(J.  A.  Rose,  Dissert.  1902.) 

Sol.  in  10  pts.  glycerine.    (Hager.) 

100  pts.  glycerine  (sp.  gr.  1.26  at  15.5°) 
dissolve  pts.  H3BO3  at  t°. 


t 

Pts. 
HaBOs 

t° 

Pts. 
H3B03 

t 

Pts. 
H3B03 

0 
10 
20 
30 

20 
24 
28 
33 

40 
50 
60 
70 

38 
44 
50 
56 

80 
90 
100 

61 

67 

72 

(Hooper,  Ph.  J.  Trans.  (3)  13.  258.) 

Solubility  of  H3BO3  in  glycerine -f  Aq  at  25°. 

G  —  g.  glycerine  in  100  g.  glycerine+Aq. 

H3BO3  =  Millimols  H3BO3  in  100  cc.  of  the 
solution. 


Solubility  of  H3BO3,  etc. — Continued. 


Acid 

Normality  of 
the  acid 

Normality  of 

H3BO 

Tartaric 

0.955 
1  .909 
2.51 
3.316 

0.890 
0.923 
0.962 
1.07 

^Jier/i,  u.  aiiuig.  x»uo,  *»•*.  A\J\J.J 

The  solubility  of  H3BO3  in  H2O  is  increased 
by  the  presence  of  racemic  acid. 


Millimols  racemic  acid 
in  10  ccm.  of  the  solvent 


0 

6.3 
12.6 
24.7 


Millimols  boric  acid 
in  10  ccm.  of  the  solution 


9.01 

9.86 

10.46 

11.65 


(Herz,  Z.  anorg.  1911,  70.  71.) 

Solubility  of  H3BO3  in  H2O  is  increased  by 
the  presence  of  tartaric  acid. 


Millimols  tartaric  acid 
in  10  ccm.  of  the  solvent 


0 

7.5 
15 
30 


Millimols  boric  acid  in 
10  ccm.  of  the  solution 


9.01 
10.00 
10.70 
12.07 


(Herz,  Z.  anorg.  1911,  70.  71.) 
Solubility  in  oxalic  acid+Aq  at  25°. 


Millimols  oxalic  acid 
in  10  ccm.  of  the  solution 


2.97 

5.95 

13.77 


Millimols  HsBOs  in  10 
ccm.  of  the  sat.  solution 


9.01 

9.95 

10.80 

11.98 


(Herz,  Z.  anorg.  1910,  66.  93.) 

Solubility  in  H2O  is  increased  by  the  pres- 
ence of  urea,  acetone  or  propyl  alcohol.  (Bog- 
dan,  C.  C.  1903,  II.  2.) 


G 

H3BO3 

Sp.  gr. 

Readily  sol.  in  hot  glacial  acetic  aci 
Chem.  Soc.  1911,  100  (2).  720.) 
Sol.  in  250  pts.  benzene.    (Hager. 

Solubility  of  H3BO3  in  mannite+A 

d.  (Holt 

q  at  t°, 

0 
7.15 
20.44 
31.55 
40.95 
48.7 
69.2 
100 

90.1 
90.1 
90.6 
92.9 
97.0 
103.0 
140.2 
390.3 

1.0170 
1.0379 
1.0629 
1.0897 
1.1130 
1  .  1328 
1.1871 
1.2719 

Solid  phase,  H3BO3 

t° 

Mg.-mols.  in  1  1. 

t° 
30° 

Mg-mols  in  1  1. 

Mannite 

H3BO3 

Mannite 

HsBOs 

25° 

0 
0.1 
03 
0.4 
0.5 
0.6 
0.7 
0.8 
1.043 
1.409 
1.781 

0.887 
0.951 
1.015 
1.039 
1.071 
1.102 
1.142 
1.173 
1.244 
1.404 
1.521 

0 
0.1 
0.2 
0.3 
0.4 
0.5 
0.6 
0.7 

1.025 
1.056 
1.086 
1.118 
1.157 
0.193 
1.21.9 
1,258 

(Herz,  Z.  anorg.  1905,  46.  268.) 

Solubility  of  H3BO3  in  organic  acids  +Aq  at 
26°. 

Acid 

Normality  of 
the  acid 

Normality  of  HsBO, 

Acetic 

0.570 
2.85 
5.70 

0.887 

0.538 
0.268 

BORATE,  AMMONIUM 


101 


Buferibuftori  bel\ie8n-HF~-f  Aq  and  amyl 
alcohol  at  25°. 

Solid  phase,  mannite 

Mg.  mols 

.mil. 

c  =  HF  concentration  (millimols)  . 

t 

a  =  H3BO3  concentration  in  alcohol  layer 
(expressed  in  millimols). 

Mannite 

H3B03 

25° 

1.075 
1  .  1424 

0 
0.2646 

w  =  H3BO3    concentration   in   water   layer 
(expressed  in  millimols). 

.259 

0.463 

c 

a 

w 

ofic 

0    ^Q 

.  ^u«_ 

.354 

\J  .  OOi7 

0.794 

500 

14.3 

71.2 

.409 

0.927 

a 

19.2 

99.2 

.536 

1.243 

a 

25.3 

144.2 

.781 

1.521 

(t 

114.3 

979.0 

OKfl 

on    i 

1  A  A      K 

(Ageno  and  Valla,  1st. 

Ven. 

(VIII)  14.  331.) 

^OU 

(( 

oU  .  1 

37.0 

L'±f±  .  O 

194.8 

H 

56.8 

321.5 

U 

108.0 

652.0 

125 

39.0 

170.5 

Distribution  between  H2O  and  amyl  alcohol 

a 

47.2 

214.0 

at  25°. 

a 

52.8 

240.5 

w  =  concentration  of 
expressed  in  millimols. 

H3BO3  in  H2O  layer 

u 

62.5 

tt 

96.0 
30.4 

on    A 

442.0 
111.2 

mo 

a  =  concentration  of  H3BO3  in  alcohol  layer 
expressed  in  millimols. 

a 

OVJ  .  '± 

65  (68?) 
90.0 

.  O 

272.8 
362.2 

w 

a 

(Abegg,  Z.  anorg.  1903,  35.  131.) 

265 

.8 

76.6 

See  also  Boron  Zn'oxide. 

196 

.5 

59.5 

159 
126 

.6 

47.5 
37.1 

Pyrobonc  (tetrabonc)  acid,  H2B4O7. 

87 

q 

33.2 

Sol.  in  H2O. 

O  1 

75 

.  <y 

.2 

22^7  •   f'J<'? 

Sp.  gr.  of  solutions  of  boric  acid,  calculated 

64 

.6 

19.76 

as  H2B4O7,  containing— 

6.3         1.27          1.91         2.54%H2B4O7 

(Abegg,  Z.  anorg.  1903,  35.  130.) 

1.0034     1.0069     1.0106     1.0147  sp.gr. 

Sat.  solution  at  15°  has  sp.  gr.  1.015.    (Ger- 

lach,  Z.  anal.  28.  473.) 

Partition  of  H3BO3  between  water  and 
mixtures  of  amyl  alcohol  and  CS2. 

Insol.   in  hot  glacial  acetic  acid.     (Holt, 
Chem.  Soc.  1911,  100.  (2)  720.) 

W  =  Millimols  H3BO3  in  10  ccm.  of  the 
aqueous  layer. 

G  =  Millimols  H3BO3  in  10  ccm.  of  the 
amyl  alcohol — CS2  layer. 


Composition  of  the 
solvent  mixture 

G 

w 

W,G 

75%  by  vol.  amyl 
alcohol  +25%  by 
vol.  CS2 

0.145 
0.275 
0.429 
0.589 

0.624 
1.198 
1.844 
2.565 

4.31 
4.36 
4.30 
4.45 

50%  by  vol.  amyl 
alcohol  + 
50%  by  vol.  CS2 

0.145 
0.259 
0.364 
0.555 

0.756 
1.353 
1.946 

2.889 

5.47 
5.21 
5.34 
5.22 

25%  by  vol.  amyl 
alcohol  + 
75%  by  vol.  CS2 

0.085 
0.175 
0.264 
0.384 

0.699 
1.467 
2.165 
3.129 

8.24 
8.40 
8.12 
8.14 

(Herz.  Z.  Elektrochem.  1910,  16.  870.) 

Borates. 

No  borate  is  quite  insol.  in  H2O;  the  alkali 
borates  are  very  sol.  The  less  sol.  borates  are 
easily  decomp.  by  H2O;  the  easily  sol.  salts 
are  also  decomp.,  but  less  quickly.  The  less 
sol.  borates  are  easily  sol.  in  H3BO3,  HNO3, 
etc.  They  are  more  sol.  in  H2O  containing 
tartaric  acid  or  potassium  tartrate  than  in 
pureH2O.  (Souberain.)  The  normal  borates 
of  the  alkaline-earths  are  sol.  to  no  inconsid- 
erable extent  in  H2O,  and  more  readily  in  hot, 
than  in  cold  H2O.  (Berzelius,  Fogg.  34.  568.) 

All  borates  are  insol.,  or  si.  sol.  in  alcohol. 

Aluminum  borate,  2A12O3,  B2O3. 

Min.  JeremciewUe. 

+3H20.    Ppt.    (Rose,  Fogg.  91.  452.) 

3A12O3,  B2O3.  Crystallized.  Insol.  in 
HNO3+Aq.  (Ebelmen,  A.  ch.  (3)  33.  62.) 

3A1203,  2B203+7H20.    Ppt.    (Rose,  l.j.) 

Ammonium  borate. 

The  system  (NH4)2O,B2O3,H2O  at  60°  has 


102 


AMMONIUM 


2(NH4)2O,4B2O3+5H2O.    (Sborgi.) 

Ammonium  diborate. 

Difficultly  sol.  in  acetone.  (Naumann.  B. 
1904,  37.  4328.) 

Ammonium  te/raborate,  (NH4)2B4O7+4H2O, 
or  perhaps  NH4H(BO2)2  +  1^H2O. 

Sol.  in  12  pts.  cold  H2O;  decomp.  by  heat. 
(Rammelsberg,  Pogg.  90.  21.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014.) 

+H2O.    (Arfvedson.) 

Ammonium  octoborate,  (NH4)2B8Oi3+6H2O. 

Sol.  in  8  pts.  cold,  decomp.  by  boiling  H2O. 
(Rammelsberg,  Pogg.  90.  21.) 

+4H2O. 

Min.  Lirdellerite.  Sol.  in  H2O  with  de- 
comp. 

Ammonium  cte/caborate,  (NH4)2B10O16+ 
6H2O. 

Permanent.    Sol.  in  H2O.    (Rammelsberg.) 
+8H2O.      (Atterberg,    Bull.    Soc.    (2)    22. 
350.) 

Ammonium  dodefcaborate,  (NH4)2Bi2O19  + 
9H2O. 

Sol.  in  hot  H2O.  (Bechi,  Sill.  Am.  J.  (2) 
17.  129.) 

Ammonium  perborate,  NH4BO3. 
See  Perborate,  ammonium.       * 

Ammonium  calcium  borate,  (NH4)8CaB4On 
=  CaB407+4(NH4)20. 

(Ditte,  C.  R.  96.  1663.) 
Ammonium  magnesium  borate. 

Sol.  in  H2O,  decomp.  by  boiling.  (Ram- 
melsberg, Pogg.  49.  451.) 

Ammonium  zinc  borate,  4(NH4)2B4O7, 

Zn(BO2)2+5H20. 
(Ditte,  C.  R.  96.  1663.) 

Barium  borate,  Ba(BO2)2. 

Ppt.    (Ouvrard,  C.  R.  1906,  142.  283.) 
+2H2O.    (Atterberg.) 
+4H2O.    (Benedikt,  B.  7.  703.) 
Sol.  in    3,300  pts.  45%  alcohol. 

7,800     "    50 
"     25,000     "    60 
55,000     "    75 
(Berg,  Z.  anal.  16.  25.) 

+  10H2O.  SI.  sol.  in  cold,  more  readily  in 
hot  H2O,  especially  in  presence  of  ammonium 
salts.  (Berzelius,  Pogg.  34.  568.)  Sol.  in 
sodium  citrate+Aq.  (Spiller.)  Insol.  in 
wood  spirit.  (Ebelmen.) 

2BaO,B2O3.  Decomp.  by  H2O  forming 
BaO,  B2O3+4H20.  (Ouvrard,  C.  R.  1906, 
142.  283.) 


.  3BaO,  B203.  Easily  sol.  in  mineral  acids. 
SI.  attacked  by  dil.  acetic  acid.  (Ouvrard, 
C.  R.  1901,  132.  258.) 

BaB4O/.  Slowly  sol.  in  warm  dilute  HNO3 
+Aq.  (Ditte,  C.  R.  77.  892.) 

+5H2O.  Sol.  in  100  pts.  cold,  and  more 
freely  in  hot  H2O.  When  freshly  pptd.  sol. 
in  cold  NH4Cl+Aq  (Wackenroder,  A.  41. 
315);  NH4NO3+Aq  (Brett,  Phil.  Mag.  (3)  10. 
96);  and  BaCl2+Aq  (Rose). 

BaB6Oio+13H2O.  (Laurent,  A.  ch.  (2)  67. 
215.) 

Ba2B2O5.     (Bloxam,  Chem.  Soc.  14.  143.) 

5BaO,  2B2O3. 

Ba3Bi<,Oi8+6H2O.  Sol.  in  100  pts.  cold 
H2O.  Easily  sol.  in  ammonium  nitrate,  or 
chloride,  or  barium  chloride +Aq.  (Rose, 
Pogg.  87.  1.) 

Ba2B6On.    Easily  sol.  in  warm  dilute  acids. 

+6H2O. 

+7H20. 

+  15H2O.    (Laurent,  A.  ch.  (2)  67.  215.) 

Barium  borate  bromide,  3BaO,  5B2O3,  BaBr2. 
(Ouvrard,  C.  R.  1906,  142.  283.) 

Barium  borate  chloride,  3BaO,5B2O3,BaCl2. 

Unaffected  by  H2O.  Sol.  in  acids.  (Ouv- 
rard, C.  R.  1906,  142.  283.) 

Bismuth  borate,  BiBO3+2H2O. 

Ppt.  SI.  sol.  in  H2O.  Decomp.  by  H2S. 
Not  decomp.  by  KOH+Aq.  (Vanino,  J.  pr. 
1906,  (2)  74.  152.) 

Cadmium  borate,  Cd3(BO3)2. 

Insol.  in  H2O,  easily  sol.  in  dil.  acids.  (Ouv- 
rard, C.  R.  1900,  130.  174.) 

Cd(BO2)2.  Difficultly  sol.  in  H2O  (Strom- 
eyer);  insol.  in  H2O,  sol.  in  HCl+Aq  (Odling); 
easily  sol.  in  warm  NH4Cl+Aq  (Rose). 

(Guertler,  Z.  anorg.  1904,  40.  242.) 

3CdO,  2B2O3+3H2O.  Ppt.  SI.  sol.  in 
H2O.  (Rose,  Pogg.  88.  299.) 

CdO,  2B2O3+2H2O.  (Ditte,  A.  ch.  1883, 
(5)  30.  255.) 

CdO,  4B2O3  +  10H2O.  Sol.  in  H2O;  de- 
comp. on  heating.  (Ditte,  A.  ch.  1883,  (5)  30. 

Cadmium    borate    bromide,    6CdO.    8B2O3, 
CdBr2. 

Insol.  in  H2O  and  fuming  HC1  or  HBr  +  Aq. 
(Rousseau  and  Allaire,  C.  R.  1894,  119.  72.) 

Cadmium    borate    chloride,    6CdO.    8B2O3, 
CdCl2. 

(Rousseau  and  Allaire,  C.  R.  1894,  118. 
1256.) 

Cadmium  borate  iodide,  6CdO,  8B2O3,CdI2. 
(Allaire,  C.  R.  1898,  127.  557.) 

Caesium  borate,  Cs2B6O]0. 

Very  sol.  in  H2O,  less  in  alcohol.  (Reischle, 
/.  anorg.  4.  116.) 


BORATE,  CUPROUS 


103 


Calcium  borate,  Ca(BO2)2. 

SI.  sol.  in  H20;  insol.  in  alkali  chlorides,  or 
boiling  cone,  acetic  acid+Aq;  sol.  in  cold  or 
hot  solutions  of  ammonium  salts,  especially 
ammonium  nitrate,  in  CaCl2+Aq,  and  also 
easily  sol.  in  dilute  mineral  acids  at  50°. 
(Ditte,  C.  R.  80.  490,  561.) 

+2H2O. 

+4H2O;  two  modifications  of  which  one 
is  very  unstable,  (van't  Hoff  and  Meyer- 
hoffer,  A.  1906,  351.  101.) 

+6H2O.  When  warmed  in  H2O  it  goes 
over  into  CaB2O4+4H2O.  (van't  Hoff  and 
Meyerhoffer.) 

Sol.  in  H2O  without  decomp.;  1  1.  solution 
contains  2  g.  salt.  (Ditte,  C.  R.  96.  1663.) 

CaB4O7.  Decomp.  by  H2O.  (Blount,  C.  N. 
54.  208.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

+3H2O.    (Ditte,  C.  R.  96.  1663.) 

+4H2O.    Min.  Bechilite. 

+6H2O.    Min.  Borocaldte.     Sol.  in  acids. 

CaB6O10,+4H2O. 

+8H2O.  Unstable.  On  standing  in  the 
solution  in  which  it  is  formed  it  changes  into 
CaB6O10+4H20. 

+  12H2O.  Unstable.  Goes  over  into 
CaB6O10+8H2O.  (van't  Hoff  and  Meyer- 
hoffer, A.  1906,  351.  104.) 

CaB8O13  +  12H2O.    (Ditte,  C.  R.  96.  1663.) 

2CaO,B2O3.  Insol.  in  H2O,  sol.  in  dil.  acids. 
(Ouvrard,  C.  R.  1905,  141.  353.) 

Ca2B6Oa.    (Ditte,  C.  R.  77.  785.) 

+3H2O.  Min.  Pandermite,  Priceite.  See 
4CaO,  5B2O3+9H2O. 

+5H2O.    Min.  Colemanite. 

If  all  the  Ca  is  in  form  of  colemanite,  the 
solution  contains  in  100  g.,  4.8  g.  H3BO3  and 
0.1  g.  CaO.  (van't  Hoff,  B.  A.  B.  1907,  653.) 

+7H20. 

+9H2O.  (van't  Hoff  and  Meyerhoffer,  A. 
1906,  351.  101.) 

3CaO,  B2O3.  Easily  sol.  in  dil.  acids. 
(Ouvrard,  C.  R.  1901,  132.  258.) 

3CaO,  5B2O3+9H2O.  (van't  Hoff,  B.  A.  B. 
1906,  II.  568.) 

4CaO,  5B2O3+9H2O.  True  composition  of 
Pandermite.  (van't  Hoff,  B.  A.  B.  1906,  II. 
572.) 

Calcium  iron  (ferrous)  borate  silicate, 

Ca2FeB2Si2O10. 
Min.  Homilite.    Easily  sol.  in  HCl+Aq. 

Calcium  magnesium  borate,  CaO,  MgO, 
3B2O3+6H2O. 

Min.  Hydroboradte.  Somewhat  sol.  in  H2O. 
Easily  sol.  in  warm  HCl+Aq  or  HNO3  +Aq. 

3CaO,  3MgO,  4B2O3.  (Ditte,  C.  R.  77. 
894.) 

Calcium  sodium  borate,  2CaO,  Na2O,  5B2O3 

+8H2O. 

(van't  Hoff,  B.  A.  B.  1907,  303. 
Ca3B10Oi8,  Na3B5O9  +  15,  or  24H2O. 


Min.  Natroborocalcite,  Ulexite.  Decomp. 
by  boiling  with  H2O.  Sol.  in  acids. 

Ca2Na4Bi2O22  +  15H2O.  Min.  Franklan- 
dite.  SI.  sol.  in  H2O;  easily  sol.  in  HC1,  and 
HNO3+Aq. 

Calcium  borate  bromide,  3CaO,  3B203,  CaBr2. 

SI.  attacked  by  H2O.  Very  sol.  in  dilute 
acetic  acid.  (Ouvrard,  C.  R.  1905, 141.  1023.) 

3CaO,  5B2O3,  CaBr2.  Hardly  attacked  by 
cold  H2O  or  very  dil.  acetic  acid.  Sol.  in 
strong  acids,  even  when  dilute.  (Ouvrard, 
C.  R.  1905,  141.  1023.) 

Calcium  borate  chloride,  Ca3B2O6,  CaCl2. 

Decomp.  quickly  by  moist  air  or  H2O, 
slowly  by  absolute  alcohol.  (Chatelier,  C.  R. 
99.  276.) 

3CaO,  3B2O3,  CaCl2.  (Ouvrard,  C.  R. 
1905,  141.  353.) 

3CaO,  5B2O3,  CaCl2.  SI.  attacked  by  cold 
H2O  and  dil.  acetic  acid+Aq.  Strong  acids 
dissolve  even  when  very  dilute.  (Ouvrard, 
C.  R.  1905,  141.  352.) 

Calcium  borate  silicate,  2CaO,  B2O3,  2SiO2 
+H20. 

Min.  Datolite.  Sol.  in  HCl+Aq  with  sep- 
aration of  gelatinous  silica. 

+2H2O.    Min.  Botryolite. 

CaO,  B2O3,  SiO2.  Min.  Danburite.  Very 
si.  attacked  by  HCl+Aq  before  ignition. 

Chromous  borate. 

Precipitate.  Sol.  in  free  acids;  insol.  in 
borax +Aq.  (Moberg.) 

Chromic  borate,  7Cr2O3,  4B2O3. 

Insol.  in  H2O;  sol.  in  excess  of  borax +Aq. 
(Hebberling,  C.  C.  1870.  122.) 

Chromic  magnesium  borate,  3Cr2O3,  6MgO, 
2B203. 

Not  attacked  by  acids.  (Ebelmen,  A.  ch. 
(3)  33.  52.) 

2Cr2O3,  9MgO,  3B2O3.  (Mallard,  C.  R. 
105.  1260.) 

Cobaltous  borate,  3CoO,  2B2O3+4H2O. 
SI.  sol.  in  H2O.    (Rose,  Pogg.  88.  299.) 
3CoO,  B2O3.     (Mallard,  C.  R.  105.  1260.) 
2CoO,  B2O3.     (Ouvrard,  C.  R.  1900,  130. 

337.) 

Cobaltous    borate    bromide,    6CoO,    8B2O3, 

CoBr2. 
(Rousseau  and  Allaire,  C.  R.  1894, 119.  73.) 

Cobaltous    borate    chloride,    6CoO,    8B2O3, 

CoCl2. 

(Rousseau  and  Allaire,  C.  R.  1894,  118. 
1257.) 

Cobaltous  borate  iodide,  6CoO,  8B2O3,  CoI2. 

(Allaire,  C.  R.  1898,  127.  557.) 
Cuprous  borate,  3Cu2O,  2B2O3. 

(Guertler,  Z.  anorg.  1904,  38.  459.) 


104 


BORATE,  CUPRIC 


Cupric  borate. 

Composition  depends  on  temperature  and 
concentration  of  solutions.  Boiling  H2O  dis- 
solves out  all  the  boric  acid.  Sol.  in  acids; 
slowly  sol.  in  hot  cone.  NH4Cl+Aq. 

Cu(BO2)2.  Insol.  in  cold  dil.  acids,  even 
HF.  Slowly  sol.  in  hot  cone.  HC1.  Not  at- 
tacked by  alkalies  or  alkali  carbonates +Aq. 
(Guertler,  Z.  anorg.  1904,  38.  456.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,42.3790.) 

Cupric   borate   ammonia,   CuB4O7,    4NH3  + 

6H20. 

Efflorescent.  Can  be  recrystallized  from  a 
little  NH4OH+Aq.  (Pasternack,  A.  151. 

227.) 

Didymium  borate,  DiBO3. 

Insol.  in  H2O  acidulated  with  HCl+Aq. 
(Cleye,  Bull.  Soc.  (2)  43.  363.) 

Di2(B4O7)3.  Insol.  in  H2O;  sol.  in  acids. 
(Frerichs  and  Smith,  A.  191.  355.) 

Glucinum  borate,  basic,  5G1O,  B2O3. 

Insol.  in  H2O;  sol.  in  acids.  (Kriiss  and 
Moraht,  B.  23.  735.) 

Iron  (ferrous)  borate. 

Ppt.  H"2O  dissolves  out  all  the  boric  acid. 
(Tiinnerman.) 

Iron  (ferric)  borate,  Fe2(BO2)6+3H2O. 
Ppt.    Insol.  in  H2O. 
Min.  Lagonite.    Sol.  in  acids. 
2Fe2O3,  3B203.    (Mallard,  C.  R.  105.  1260.) 
6Fe2O3,  B2O3+6H2(X    Ppt.     (Rose,  Pogg. 

9Fe26s,  B2O3+9H2O.    Ppt,    (Rose.) 

Iron  (ferric)  magnesium  borate,  3Fe2O3, 
6MgO,  2B203. 

Insol.  in  H2O.  Sol.  in  cone.  HCl+Aq 
(Ebelmen,  A.  ch.  (3)  33.  53.) 

2Fe2O3,  9MgO,  3B2O3.  (Mallard,  C.  R. 
105.  1260.) 

Iron  (ferroferric)  magnesium  borate,  3MgO. 

FeO,  Fe203,  B2O3. 

Min.  Ludwigite.  Slowly  sol.  in  HCl+Aq, 
when  finely  powdered. 

Iron  (ferrous)  borate  bromide,  6FeO,  8B2O3, 
FeBr2. 

Slowly  sol.  in  hot  HNO3+Aq.  (Rousseau 
and  Allaire,  C.  R.  116.  1445.) 

Iron  (ferrous)  borate  chloride,  6FeO,  8B2O3, 
FeCl2. 

Slowly  sol.  in  hot  HNO3+Aq.  (Rousseau 
and  Allaire,  C.  R.  116.  1195.) 

Lanthanum  borate,  2La2O3,  B2O3. 
(Nordenskjold,  Pogg.  114.  618.) 
La2(B4O7)3.    Ppt.    (Smith.) 
Formula  is  La2B6O15+zH2O.     (Cleve    B 


Lead  borate,  basic, 

2PbO,  B2O3+2H,O.    Ppt. 

4PbO,  3B2O3+4H2O.    Ppt. 

+5H2O.    Ppt. 

6PbO,  5B2O3+6H2O.    Ppt. 

8PbO,  3B2O3+8H2O.    Ppt. 

9PbO,  5B2O3+9H2O.  Ppt..  (Rose,  Pogg 
87.  470.) 

Lead  borate,  Pb(BO2)2+H2O. 

Insol.  in  H2O.  Easily  sol.  in  dil.  HNO3,  or 
boiling  HC2H3O2+Aq.  Decomp.  by  H2SO4, 
HC1,  also  by  boiling  KOH,  or  NaOH+Aq. 
Insol.  in  alcohol.  (Herapath,  Phil.  Mag.  (3) 
34.  375.) 

Sol.  in  NH4Cl+Aq;  sol.  in  sat.  NaCl+Aq,. 

2PbO,  3B2O3+4H20.    (Herapath.) 

PbB4O7+4H2O.  Slightly  sol.  in  pure  H2O, 
but  insol.  in  solutions  of  Na  salts  as  Na2B4O7 
+Aq.  (Soubeiran.) 

Lead  borate  chloride,  Pb(BO2)2,  PbCl2+H20. 
Insol.  in  cold,  very  slowly  decomp.  by  hot 
H2O  into  its  constituents.  Easily  sol,  in  dil. 
hot  HNO3+Aq;  insol.  in  alcohol.  (Herapath, 
Phil.  Mag.  (3)  34.  375.) 

Lead  borate  nitrate,  Pb(BO2)2,  Pb(NO3)2  + 

H2O. 
Insol.  in  alcohol.    (Herapath.) 

Lithium  borate,  LiBO2. 

Solubility  in  HoO. 
100  g.  H20  dissolve  g.  LiB02  at  t°. 


t° 

g.  LiB02 

t 

g.  LiBO- 

0 

0.7 

30 

4.9 

10 

1.4 

40 

11.12 

20 

2.6 

45 

20. 

(Le  Chatelier,  C.  R.  1897,  124.  1094.) 

Insol.  in  acetone.     (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 
Insol.  in  methyl  acetate.     (Naumann,  B. 

1909,  42.  3790.) 

Insol.   in   ethyl   acetate.      (Naumann,    B. 

1910,  43.  314.) 

+8H20.     (Le  Chatelier,  Bull.  Soc.  1899, 

+  16H2O.  Effloresces  in  the  air;  slowly 
sol.  in  cold  H2O,  rapidly  in  hot  H2O.  (Le 
Chatelier,  C.  R.  1897,  124.  1092.) 

Li2H4(BO3)2  +  14H2O.    (Reischle,  Z.  anorg. 

4»    lot)./ 

Li2B4O7.  Deliquescent;  easily  sol.  in  H2O. 
(Arfvedson,  A.  ch.  10.  82.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014.) 

Insol.  in  acetone.    (Naumann,  B.  1904,  37. 

Insol.  in  methyl  acetate.     (Naumann,  B. 

+5H2O.  Insol.  in  alcohol.  (Filsinger, 
Arch.  Ph.  (3)  8.  198.) 


BORATE,  MOLYBDENUM 


105 


Li2O,  3B2O3+6H2O.  Very  sol.  in  H,O; 
insol.  in  alcohol.  (Filsinger.) 

Li2C,  4B2O3.  Insol.  in  H2O.  (Le  Chatelier, 
Bull.  Soc.  1899,  (3)  21.  35.) 

+  10H2O.  Sol.  in  H2O;  insol.  in  alcohol. 
(Filsinger.) 

"  Acid  lithium  borate"  is  less  sol.  than  the 


tetraborate.    (Gmelin.) 

Li2O,    5B2O3  +  10H2O. 
1908.  1089. 


(Dukelski,   C.   A. 


Magnesium  borate,  Mg(BO2)2. 

(Ditte,  C.  R.  77.  893.) 

+3HoO.    Min.  Pinnoile. 

+4H2O.     (Laurent,  A.  ch.  (2)  67.  215.) 

-j-8H2O.  Insol.  in  cold  or  hot  H2O;  easily 
sol.  in  HCl+Aq.  Decomp.  by  cone.  HC1 
+Aq  into  H3BO3  and  MgCl2.  (Wohler.) 

MgB4O7+8H2O.    (Popp,  A.  Suppl.  8.  1.) 

MgO,  3B2O3+8H2O.  Very  slowly  sol.  in 
H2O.  (Rose,  A.  84.  221.) 

Sol.  in  75  pts.  cold  H2O.  (Rammelsberg, 
Pogg.  49.  445.) 

2MgO,  BoO3.  Insol.  in  H2O,  but  sol.  in 
NaoCO3+Aq.'  (Guertler,  Z.  anorg.  1904,  40. 
236.) 

+HoO.  Very  si.  sol.  in  l/io  N  HCl+Aq. 
(van't  Hoff,  B.  A.  B.  1907,  658.) 

Min.  Ascharite. 

3MgO,  B2O3.  Insol.  in  H2O;  easily  sol.  in 
acids.  (Ebelmen,  A.  80.  208.) 

Very  si.  sol.  in  cold,  but  somewhat  decomp. 
by  boiling  H2O.  (Rammelsberg.) 

+9H>O.  Somewhat  sol.  in  cold  H2O. 
(Wohler,  Pogg.  28.  525.) 

3MgO,  2B2O3.  Sol.  in  warm  H2SO4  or 
HNO3+Aq.  (Ditte,  C.  R.  77.  893.) 

MgO,  6B2O3  +  18H20  =  Mg(BO2)2,  10HBO2 
+  13H2O.  (Rammelsberg,  Pogg.  49.  445.) 

3MgO,  4B2O3.  Sol.  in  hot  dil.  acids;  insol. 
in  acetic  acid.  (Ditte,  C.  R.  77.  893.) 

5MgO,  2B2O3  +  1K,  and  3H2O.  Min. 
Szzibelyite.  Difficultly  sol.  in  HCl+Aq. 

9MgO,  B2O3.     (Mallard,  C.  R.  106.  260.) 

Magnesium  manganous   borate,   3Mg2B2O5, 

4Mn2B2O6+7H2O. 
Min.  Xussexite.    Sol.  in  HCl+Aq. 

Magnesium  potassium  borate,  KMg2BuOi9  + 
9H20. 

Min.  Kaliborite.  Insol.  in  H2O.  (Feit, 
Ch.  Z.  1889,  13.  1188.) 

2MgO,  2K2O,  11B2O3+20H2O.  (van't 
Hoff  and  Lichtenstein,  B.  A.  B.  1904,  936.) 

Magnesium  sodium  borate,  Mg2B6On, 

Na2B4O7+30H2O. 

Efflorescent.  About  as  sol.  in  cold  H2O  as 
borax;  solution  separates  out  a  Mg  borate 
on  warming,  which  redissolves  on  cooling. 
Decomp.  by  boiling  H2O.  (Rammelsberg.) 

Magnesium  strontium  borate,  3MgO,  3SrO 

4B2O3. 
Easily  sol.  in  dil.  acids.     (Ditte,  C.  R.  77. 

.895.) 


Magnesium    borate     bromide,     2Mg3B8Oi5, 

MgBr2  or  6MgO,  8B2O3,  MgBr2. 
(Rousseau  and  Allaire,  C.  R.  1894,  119,  71.) 

Magnesium  borate  chloride,  2Mg3B8Oi5, 
MgCl2. 

Min.  Boradte.  Insol.  in  H2O;  slowly  sol. 
n  acids.  (Kraut.) 

Stassfurthite.  Easily  sol.  in  warm  acids. 
;Bischof.) 

Magnesium  borate  iodide,  6MgO,  8B2O3, 
MgI2. 

(Allaire,  C.  R.  1898,  127.  556.) 

Magnesium    borate    phosphate,    Mg(BO2)2, 

2MgHPO4+7H2O. 
Min.  Luneburgite. 

Magnesium  borate  sulphate,  2Mg3B4O9, 
3MgSO4+12H2O. 

Min.  Magnesium  sulphoborite. 

Sol.  in  mineral  acids  when  ground.  (Nau- 
pert,  B.  1893,  26.  874.) 

Manganous  borate,  MnB4O7  (?). 

Insol.  in  H2O  (Berzelius);  very  si.  sol.  in 
H2O  (Thomas,  Am.  Ch.  J.  4.  358);  decomp. 
by  warm,  slowly  by  cold  H2O.  Sol.  in  MgSO  \ 
+Aq  (Berzelius). 

+3H2O.  (Endemann  and  Paisley,  Zeit. 
angew.  Ch.  1903,  16.  176.) 

+5H2O.     Ppt.     (Endemann  and  Paisley.) 

Very  hydroscopic.  (Endemann,  Am.  Ch. 
J.  1903,  29.  72.) 

3MnO,  B2O3.    (Mallard,  C.  R.  106.  1260.) 

Not  attacked  by  H2O.  Very  sol.  in  acids. 
(Ouvrard,  C.  R.  1900,  130.  336.) 

3MnO,  2B2O3.     (Mallard.) 

MnH4(BO3)2.    Very  si.  sol.  in  H2O. 

Solubility  in  2%  Na2SO4+Aq.  At  18.5°, 
0.77  g.  MnH4(BO3)2  are  dissolved  per  litre; 
at  40°,  0.65  g.;  at  60°,  0.36  g.;  at  80°,  0.12  g. 

Solubility  in  2%  NaCl+Aq.  1  1.  solution 
dissolves  1.31  g.  salt  at  18.2°;  0.6  g.  at  59°; 
and  0.29  g.  at  80°. 

Solubility  in  2%  CaCl2+Aq.  1  1.  CaCl2  + 
Aq  dissolves  2.91  g.  salt  at  17.6°;  2.44  g.  at 
43.0°;  2.25  g.  at  61°;  and  1.35  g.  at  80°.  (Hart- 
ley and  Ramage,  Chem.  Soc.  63.  129.) 

Manganous  borate  bromide,  6MnO,  8B2O3, 

MnBr2. 
(Rousseau  and  Allaire,  C.  R.  1894, 119.  73.) 

Manganous  borate  chloride,  6MnO,  8B2O3, 

MnCl2. 
(Rousseau  and  Allaire,  C.  R.   1894,  118. 

1257.) 

Molybdenum  borate,  MoO2,  2B2O3  (?). 

Insol.  in  H2O;  sol.  in  H3BO3+Aq.  (Ber- 
zelius.) 


106 


BORATE,  MOLYBDENUM 


Molybdenum  borate,  Mo2O3,  B2O3. 

Precipitate.  Insol.  in  H2O;  si.  sol.  in  a 
solution  of  boric  acid.  (Berzelius.) 

See  Boromolybdic  Acid. 

Nickel  borate,  Ni(BO2)2+2H2O. 

Insol.  in  H2O.  Easily  sol.  in  acids.  Easily 
sol.  in  warm  NH4Cl+Aq.  (Rose,  Pogg.  88. 
299.) 

2NiO,  B2O3+zH2O.  Easily  sol.  in  acids. 
(Rose.) 

3NiO,  2B2O3+5H2O.  Easily  sol.  in  acids. 
(Rose.) 

3NiO,B2O3.  Not  attacked  by  H2O;  sol.  in 
acids.  (Ouvrard,  C.  R.  1900,  130.  337.) 

Nickel  borate  bromide,  6NiO,  8B2O8,  NiBr2. 
(Rousseau,  C.  R.  1894,  119.  73.) 

Nickel  borate  chloride,  6NiO,8B2O3,NiCl2. 
(Rousseau,  C.  R.  1894,  118.  1257.) 

Potassium  borates. 

Solubility  of  B2O3  in  K2O+Aq  at  30°. 


Solution  contains 

%  by  wt.  K20 

%  by  wt.  B2O 

Solid  phase 

47.50 

KOH,  2H2O 

46.45 

'  0.72 

it 

46.36 

0.91 

K2O,  B2O3,  2.5H2O 

40.51 

1.25 

« 

36.82 

1.80 

a 

36.72 

1.85 

u 

32.74 

3*51 

n 

29.63 

6-98 

u 

26.89 

12.12 

11 

24.84 

17.63 

" 

23.30 

18.19 

K2O,  2B2O3,  4H2O 

16.21 

13.10 

« 

11.78 

9.82 

u 

9.18 

8.00 

" 

6.22 

9.13 

« 

7.79 

13.20 

u 

7.73 

13.37 

K2O,  2B2O3,  4H2O  + 

K2O,  5B2O3,  8H2O 

7.81 

13.28 

7.67 

13.19 

a 

7.71 

13.21 

K2O,  5B2O3,  8H2O 

7.63 

13.28 

« 

3.42 

7.59 

« 

1.80 

4.15 

« 

0.80 

3.05 

n 

0.51 

3.19 

a 

0.33 

4.58 

K2O,  5B2O3,  8H2O  + 

B(OH)3 

0.38 

4.51 

« 

0.31 

4.46 

« 

0.28 

4.36 

B(OH)3 

3.54 

n 

At  30°  only  the  three  potassium  borates 
K2O,  B2O3+2.5H2O;  K2O,  2B2O3+4H2O  and 

K2O,  5B2O3+8H2O  exist  in  stable  form. 

(Dukelski,  Z.  anorg.  1906,  50.  42.) 

Potassium  raetaborate,  KBO^. 

Sol.  in  small  amount  of  H2O.  (Berzelius, 
Pogg.  34.  568.) 

+  1MH2O.  Only  stabile  hydrate.  (Dukel- 
ski,  Z.  anorg.  1906,  50.  42.) 

+  1HH2O.  (Atterberg,  Bull.  Soc.  (2)  22. 
350.) 

Potassium  /elaborate,  K2B4O7. 

Very  sol.  in  H2O. 

+4H2O.  (Atterberg,  Bull.  Soc.  (2)  22. 
350.) 

Only  stabile  hydrate.     (Dukelski,  I  c.) 

+5H2O.  Very  sol.  in  H2O;  more  sol.  than 
K2B6Oio  or  K2B12Oi9. 

+6H2O.  .  (Atterberg,  I.  c.) 

Potassium     Aezaborate,     K2B6Oio4-5,      and 

8H2O. 

Easily  sol.  in  H2O. 
Does  not  exist.     (Dukelski,  Z.  c.) 

Potassium  elaborate,  K2Bi0Oi6+8H2O. 
Sol.  in  H2O.     (Rammelsberg*.) 
Only  hydrate.    (Dukelski.) 

Potassium  dode/caborate,  K2Bi2Oi94-10H2O. 

81.  sol.  in  cold,  very  sol.  in  hot  H2O. 
(Laurent,  A.  ch.  67.  215.) 

=  K2BioOi6.    (Rammelsberg.) 

Does  not  exist.     (Dukelski.) 

Potassium  borate  fluoride,  KBO2,  KF. 

Sol.  in  H2O.  (Schiff  and  Sestini,  A.  228. 
72.) 

KBO2,  2KF.  Sol.  in  little,  decomp.  by 
much  H2O.  Insol.  in  H2O.  (SchuT  and  Ses- 
tini,  A.  228.  72.) 

Rubidium  borate,  Rb2B4O7. 

Anhydrous.    (Reisehle,  Z.  anorg.  4.  166.) 
+6H2O.    Not  deliquescent  or  efflorescent. 

Sol.  in  H2O.    (Reissig,  A.  127.  33.) 

Samarium  borate,  SmBO3. 

Insol.  in  H2O;  sol.  in  HCl+Aq.  (Cleve, 
Bull.  Soc.  (2)  43.  1670.) 

Scandium  borate,  ScBO3. 

Sol.  in  dil.  acids.  (Crookes,  Phil.  Trans. 
1910,  210.  A.  364.) 

Silver  borate,  AgBO2. 

81.  sol.  in  H2O.  By  washing  with  H2O  the 
boric  acid  is  dissolved  out.  (Rose.  Pharm. 
Centralbl.  1853.  205.) 

Sol.  with  decomp.  in  Na2S2O3+Aq  (Her- 
schel);  sol.  in  NH4NO3+Aq  if  pptd.  cold. 

1  1.  H2O  dissolves  ca.  6  x  10~2  gram-atoms 
at  25°.  (Abegg  and  Cox,  Z.  phys.  Ch.  1903, 
46.  11.) 

Insol.  in. ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

3Ag2O,  4B2O3.    (Rose,  L  c.) 


BORATE,  SODIUM 


107 


Sodium  borates. 

+8H2O.    (Atterberg.) 

Solubility  of  B2O3  in  Na2O+Aq  at  30C. 

+4H2O  and  +8H2O  are  the  only  hydrates 

Solution   contains 

iormed.    (Dukelski.) 
System  Na2O,  B2O3,  H2O  at  60°  investi- 

% by  wt. 

%   by  wt. 

Solid  phase 

gated  by  Sborgi.     (Real.  Ac.  Line.  1915,  (5) 

Na2O 

B2O:, 

24.  I,  443.) 

42.00 
40.85 

2.7i 

NaOH,  H2O 

u 

Sodjum  tefraborate,  Na2B4O7  (Borax). 

41.37 

5.10 

u 

100  g.  H2O  dissolve  at: 

38.85 
34.44 

5.55 
3.73 

Na2O,  B2O3,  4H2O 

5°    10°    21.5°  30°    37.5° 
1.3    1.6      2.8    3.9      5.6  g.  anhydrous  salt. 

29.39 

2.51 

" 

45°  50°  54°  55°    56°    57° 

28.61 

2.38 

tt 

8.1  10.5  13.3  14.2  15.0  16.0  g.  anhydrous  salt. 

27.78 
26.13 

2.44 
2.75 

u 

(Horn  and  van  Wagener,  Am.  Ch.  J.  1903, 

25.08 
OQ  fin 

2.98 

tt 

Insol.   in   ethyl   acetate.      (Naumann,    B. 

—  -  >  .  \j\j 
16.61 
21.58 

20.58 
18.31 

13.69 
4.63 

4.69 
4.97 

Na2O,  B2O3,  4H2O  + 
Na2O,  B2O3,  8H2O 
Na2O,  B2O3,  8H2O 

1910,  43.  314.) 
Sol.  in  amyl  alcohol  in  the  presence  of  meta- 
arsenious  acid  and  excess  of  H3BO3.     (Auer- 
bach,  Z.  anorg.  1903,  37.  358.) 
+4H20. 

i   CTJ  r\ 

15.32 

6.21 

it 

7^  Oil  2^  • 

100  g.  H2O  dissolve  at: 

13  .  25 

8  18 

12.39 

9  12 

tt 

65°    70°    80°      90°    100° 

8^85 

HK49 

Na2O,  2B2O3,  10H2O 

22.0  24.4   31.4   40.8    52.3  g.  anhydrous  salt. 

5.81 

6.94 

(Horn  and  van  Wagener,  Am.  Ch.  J.  1903, 

4.00 

4.76 

« 

30.  347.) 

1.88 

2.41 

« 

+6H2O.    Grows  opaque  in  the  air.    (Bechi, 

1.38 

5.16 

14 

Sill.  Am.  J.  (2)  17.  129.) 

1.84 

7.36 

U 

+  10H2O.    Only  stabile  hydrate.     (Dukel- 

2.02 

7.79 

tt 

ski,  Z.  anorg.  50.  30.)    Efflorescent  on  surface 

2.40 

9.48 

it 

in  dry  air.     Not  efflorescent  when  free  from 

4.08 

17.20 

Na2O,  2B2O3,  10H2O 

Na2CO3.    (Sims.) 

+Na2O,  5B2O3, 

10H2O 

Sol.  in  12  pts.  cold,  and  2  pts.  hot  H2O.     Sat.  cold 

3.79 

15.84 

Na2O,  5B2O3,  10H2O 

Na2B4O?+Aq  contains  9.23%,  and  sat.  hot  Na-jB4O7  + 
Aq  contains  33.33%  Na-^O-.     (Gmelin.) 

3.47 

13.30 

" 

Sol.  in  20  pts.  cold,  and  6  pts.  boiling  H2O.     (Wal- 

9  9fi 

19    14- 

K 

lerius.) 

—  -  —  I  ) 

1.99 

1  —  .   J.TT 

11.84 

Na2O,  5B2O3,  10H2O 

Sol.  in  15  pts.  H2O  at  18.75°.     (Abl.) 
100  pts.  H2O  at  15.5°  dissolve  5  pts.;  at  65°,  40  pts.; 

+B(OH)3 

at  100°,  166  pts.  Na2B4O7  +  10H2O.    (Ure's  Dictionary.) 

1.86 

11.78 

B(OH)3 

100  pts.  sat.  Na2B4O+Aq  at  105.5°  contain  52.5  pts. 
Na2B4O7,  or  100  pts.  H6O  dissolve  110.54  pts.  Na2B4O7, 

1.81 

11.18 

or  1  pt.  Na2B<O7  is  sol.  in  0.9047  pt.  H2O  at  105.5°. 

0.64 

6.11 

if. 

(Griffith,  Quar.  J.  Sci.  18.  90.) 

3.54 

u 

At  30°,  only  the  four  sodium  borates  Na2O, 

Solubility  in  100  pts.  H2O  at  t°. 

B2O3+4H2O;     Na2O,    B2O3+8H2O;    Na2O, 

Pts                                                Pts. 

2B2O3  +  10H2O;    and  ,Na2O,    5B2O3  +  10H2O 

exist  as  stable  phases. 

i  a?    4    7     +K)H2O                   i  a2    4    ,      -|_10H2O 

(Dukelski,  Z.  anorg.  1906,  50.  46.) 

0        1.49       2.83        60      18.09        40.43 

10        2.42       4.65        70     24.22        57.85 

Sodium  wetaborate,  NaBO2. 

20        4.05       7.88        80     31.17         76.19 

Anhydrous.    Easily  sol.  in  H2O,  with  evolu- 
tion of  heat. 

30        6.00      11.90        90     40.14       116.66 
40        8.79      17.90       100     55.16       201.43 

+H2O.    Easily  sol.  in  H2O.    (Benedikt.) 

50      12.93     27.41 

B.  7.  703.) 

+3H2O.    Easily  sol.  in  H2O.    (Berzelius.) 

+4H2O.  SI.  efflorescent.  Sol.  in  hot,  less 
sol.  in  cold  H2O.  Melts  at  57°  in  its  crystal 
H2O.  (Dukelski,  Z.  anorg.  50.  42.) 

+43^H2O.  (Atterberg,  Z.  anorg.  1906,  48. 
370.) 

+5^H2O.     (Atterberg.) 


(Poggiale,  A.  ch.  (3)  8.  46.) 

100  pts.  H2O  dissolve  1.4  pts.  Na2B4O7  at 
0°,  and  55.3  pts.  at  100°.  (Mulder.) 

Na2B4O7+Aq  sat.  at  15°  has  sp.  gr.  = 
1.0199,  and  contains  3.926  pts.  Na2B4O7  to 
100  pts.  H2O.  (Michel  and  Krafft,  A.  ch.  (3) 
41. -471.) 


108 


BORATE,  SODIUM 


Na2B4O7+Aq   sat.   at    17°   has   sp.   gr. 
1.0208.    (Stolba,  J.  pr.  97.  503.) 

Sp.  gr.  of  Na2B4O7+Aq  at  15°. 


J 

% 
NasRiCh 

+  10H20 

Sp.  gr. 

4 

% 
Na«B407 
+  10H2() 

Sp.  gr. 

1 

2 
3 

0.52 
1.06 
1.59 

1.0049 
1.0099 
1.0149 

4 
5 
6 

2.11 
2.64 
3.17 

1.0199 
1.0249 
1.0299 

(Gerlach,  Z.  anal.  28.  473.) 

Sp.  gr.  of  Na2B4O7+Aq  sat.  at  15°  =  1.032. 
(Gerlach.) 

Sat.  Na2B4O7-f  Aq  boils  at  105.5°,  and  con- 
tains 110.5  pts.  Na2B4O7  to  100  pts.  H2O. 
(Griffith.) 

Sat.  Na2B4O7+Aq  forms  a  crust  at  103°, 
and  contains  60.14  pts.  Na2B4O7  to  100  pts. 
H2O;  highest  temp,  observed,  104.3°.  (Ger- 
lach, Z.  anal.  26.  427.) 

B.-pt.  of  Na2B4O7-f-Aq  containing  pts. 
Na2B4O7  to  100  pts.  H2O. 


B.-pt. 

Pts. 
Na2B40; 

B.-pt. 

Pts. 
Na2B407 

100.5° 

8.64 

103.0° 

61.2 

101.0 

17.2 

103.5 

75.4 

101  .  5 

26.5 

104.0 

90.8 

102.0 

37.5 

104.5 

109.0 

102.5 

48.5 

104.6 

112.3 

(Gerlach,  Z.  anal.  26.  452.) 


(Til- 


M.-pt.  of  Na2B4O7  +  10H2O  is  75.5°. 
den,  Chem.  Soc.  45.  407.) 

Insol.  in  alcohol. 

100  g.  alcohol  (0.941  sp.  gr.)  dissolve  2.48  g. 
at  15.5°  (U.  S.  P.). 

Sol  in  alcoholic  solution  of  NaC2H3O2. 
(Stromeyer.) 

Sol.  in  14.7  pts.  glycerine  of  1.225  sp.  gr. 
(Vogel.) 

Sol.  in  1  pt.  glycerine.  (Schtiltze,  Arch. 
Pharm.  (3)  6.  149.) 

100  g.  glycerine  dissolve  60.3  g.  at  15.5° 

Min.  Tincal. 

Sodium  borate,  Na2B8Oi3  +  10H2O. 

Sol.  in  5-6  pts.  cold  H2O.  (Bolley,  A.  68. 
122.)  Perhaps  sodium  hydrogen  tetraborate 
NaHB407+4^H20. 

Na2B10O16  +  10H2O.  Decomp.  by  H2O. 
(Atterberg,  Z.  anorg.  48.  370.) 

Stabile.    (Dukelski,  Z.  anorg.  50.  42.) 

+  11H2O.    (Laurent,  C.  R.  29.  5.) 

Sodium  borate  fluoride,  NaBO2,  .3NaF  + 
4H2O. 

Sol.  in  H2O. 

Basarow  (B.  7.  112)  considers  this  salt  to 
be  a  mixture. 


Na2B4O7,  12NaF+22H2O.  Can  be  sep- 
arated into  its  constituents  by  H2O.  (Ber- 
zelius,  Berz.  J.  B.  23.  96.) 

Strontium  borate,  Sr(BO2)2. 

(Ditte,  C.  R.  77.  788.) 

Easily  hydrated  by  H2O  forming  SrO,'  B2O3 
+2H2O.  Very  sol.  in  dil.  acetic  acid.  (Ouv- 
rard,  C.  R.  1906,  142.  282.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.)  . 

+2H2O.    (Ouvrard,  I.  c.} 

+4H2O.     (Ouvrard,  I.  c.) 

+5H2O.  1  1.  H2O  dissolves  2.3  g.  at  10°. 
(Ditte,  A.  ch.  1883  (5)  30.  253.) 

SrB4O7.  Insol.  in  H2O;  sol.  in  dil.  acids. 
(Guertler,  Z.  anorg,  1904,  40.  243.) 

+4H2O.  Sol.  in  130  pts.  boiling  H2O.  100 
pts.  H2O  at  100°  dissolve  7.7  pts.  (Ure's  Diet.). 
Easily  sol.  in  cold  NH4  salts  +Aq;  sol.  in  cold 
HNO3+Aq. 

2SrO,B2O3.  Easily  decomp.  by  H2O  form- 
ing B2O3,  SrO,  4H2O.  Very  sol.  in  acids. 
(Ouvrard,  C.  R.  1906,  142.  282.) 

3SrO,  B2O3.  Less  easily  attacked  by  H2O 
than  Ca  comp.  Very  sol.  in  mineral  acids. 
SI.  attacked  by  dil.  acetic  acid.  (Ouvrard, 
C.  R.  1901,  132.  258.) 

SrB6Oio.  Very  si.  sol.  in  H2O;  sol.  in  acids. 
(Laurent.) 

SrB8O31+7H2O.    Ppt.    (Laurent.) 

+  12H2O.     (Ditte.) 

Sr3B4O9.  Sol.  in  cold  mineral  acids  and 
acetic  acid.  (Ditte,  C.  R.  77.  785.) 

2SrO,  3B2O3.  Easily  sol.  in  acids.  (Ditte, 
L  c.) 

Strontium    borate    bromide,    3SrO.    5B2O3, 
SrBr2. 

As  the  chloride.  (Ouvrard,  C.  R.  1906, 
142.  283.) 

Strontium    borate    chloride,    3SrO,    5B2O3, 

SrCl2. 

SI.  attacked  by  cold  H2O.  not  attacked  by 
dilute  acetic  acid.  (Ouvrard.  C.  R.  1906,  142. 

282.) 


Thallous  borate, 

Decomp.  in  the  air.  (Buchtala.  J.  pr.  1913, 
(2)  88.  784.) 

T12B2O7.     (Buchtala.) 

T12B4O7.  Ppt.  Sol.  in  boiling  H2O;  insol. 
i  n  cold  dil.  H2SO4+Aq.  (Crookes.) 

+2H2O.  (Buchtala,  J.  pr.  1913  (2)  88. 
774.) 

T12B6O10+3H2O.      (Buchtala.) 

Tl2B8Oi3+4H2O.     (Buchtala.) 

T12B10O16+8H2O.     (Buchtala.) 

T12B12O19+7H2O.     (Buchtala.) 

Thorium  borate  (?). 

Precipitate.  Insol.  in  H2O  and  H3BO3  + 
Aq.  (Berzelius.) 

Tin  (stannous)  borate  (?). 
Ppt.    (Wenzel.)    ' 


BORON  BROMIDE  PHOSPHINE 


109 


Divanadyl  borate. 

Insol.  in  H2O;  sol.  in  H3BO3+Aq.     (Ber- 

zelius.) 

Ytterbium  borate,  YbBO3. 

Insol.  in  cone.  HC1;  sol.  in  HF.  (Cleve,  Z. 
anorg.  1902,  32.  148.) 

Yttrium  borate. 

Precipitate.    (Berlin,  Pogg.  43.  105.) 

Zinc  borate,  3ZnO,  2B2O3. 

(Mallard,  C.  R.  105.  1260.) 

Decomp.  by  H2O;  very  sol.  in  dil.  acids. 
(Ouvrard,  C.  R.  1900,  130.  336.) 

ZnO,  2B2O3+4H2O.  Sol.  in  H2O  with 
decomp.  (Ditte,  A.  ch.  1883,  (5)  30.  256.) 

3ZnO,  4B2O3+H2O.  Ppt.  (Holdermann, 
Arch.  Pharm.  1904,  242.  567.) 

ZnO,  4B203  +  10H2O.  (Ditte,  A.  ch:  1883, 
(5)  30.  256.) 

9ZnO,  4B2O3+9H2O.  SI.  sol.  in  H3BO3 
+Aq.  (Rose,  Pogg.  88.  299.) 

3ZnO,  B2O3.  Insol.  in  mineral  acids,  (le 
Chatelier,  C.  R.  113.  1034.) 

Zinc  borate  ammonia,  ZnB4O7,  4NH3+6H2O. 
Easily  sol.  in  NH4OH,  HC2H3O2,  H2SO4, 
HC1,    and   HNO3+Aq.      (Biichner,   A.    151. 
234.) 

Zinc  borate  bromide,  6ZnO,  8B2O3,  ZnBr2. 
(Rousseau  and  Allaire,  C.  R.  116.  1446.) 

Zinc  borate  chloride,  6ZnO,8B2O3,ZnCl2. 

Insol.  in  HC1.  (Rousseau,  C.  R.  1894,  118. 
1256.) 

Zinc  borate  iodide,  6ZnO,  8B2O3,  ZnI2. 
(Allaire,  C.  R.  1898,  127.  556.) 

Zirconium  borate,  (?). 
Insol.  in  H2O. 

Perboric  acid. 
See  Perboric  Acid. 

Boric  phosphoric  acid. 
See  Phosphoboric  acid. 

Boric  tungstic  acid. 
See  Borotungstic  acid. 

Boric  acid  sulphur  In'oxide. 
See  Borosulphuric  acid. 

Borimide,  B2(NH)3. 

Decomp.  by  H2O;  insol.  in  all-  indifferent 
solvents;  sol.  in  liquid  NH3+S  to  form  a  dark 
blue  solution.  (Stock,  B.  1901,  34.  3044.) 

Borimide  hydrochloride,  B2(NH)3,3HC1. 

Decomp.  by  H2O;  insol.  in  all  ordinary  or- 
ganic solvents.  (Stock,  B.  1901,  34.  3045.) 


Borofluorhydric  acid,  HBF4. 
See  Fluoboric  acid. 

Borofluorides. 
See  Fluoborides. 

Boromolybdic  acid. 

Sol.  in  H2O.  Decomp.  by  alcohol.  (Ber- 
zelius.) 

Boron,  B. 

(a)  Amorphous.  Somewhat  sol.  in  pure 
H2O,  when  not  ignited.  Salts  and  acids  sep- 
arate it  out  of  aqueous  solution.  Upon  evap- 
oration of  H2O  solution  a  crust  is  formed, 
which  is  only  partially  sol.  in  H2O.  (Ber- 
zelius,  Pogg.  2.  113.)  Decomp.  by  hot  H2SO4 
and  cold  moderately  cone.  HNO3+Aq. 
Strongly  ignited  amorphous  B  is  much  less 
easily  attacked  by  reagents  than  freshly  pptd., 
and  is  insol.  in  H2O.  (Berzelius.)  Insol.  in 
caustic  alkalies +Aq;  also  in  alcohol  and  ether. 

Above  boron  was  very  impure.  (Moissan, 
C.  R.  114.  392.) 

Pure  B  is  not  attacked  by  acids,  but  has  a 
strong  reducing  action  on  KMnO4+Aq,  FeCl3 
+Aq,  etc.  (Moissan,  C.  R.  114.  617.) 

Does  not  melt  at  1500°.  Readily  sol.  in 
cone,  acids,  as  H2SO4,  HNO3,  H3PO4";  very  si. 
sol.  in  hydracids;  decomp.  H2O  at  red  heat. 
(Moissan,  A.  ch.  1895,  (7)  6.  313-14.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  827.) 

^(6)  Crystallized.  1.  Insol.  in  H2O,  HC1,  or 
KOH+Aq.  Very  slightly  and  slowly  attacked 
by  boiling  cone.  H2SO4.  Gradually"sol.  in  hot 
cone.  HNO3.  Formula  is  A12B24.  (Hampe, 

A.  183.  75.) 

2.  Very  slightly  attacked  by  cone.  HC1  or 
H2SO4;  slowly  but  completely  sol.  in  cone. 
HNO3;  insol.  in  KOH+Aq.  Formula  is 
C2A13B48.  (Hampe.) 

C2A13B44.  Crystalline.  Insol.  in  a  solution 
of  CrO3  in  H2SO4.  Insol.  in  hot  cone.  HC1 
and  H2SO4.  Sol.  in  hot  cone.  HNO3.  (Biltz, 

B.  1910,  43.  303.) 

Boron  Iribromide,  BBr3. 

Sol.  in  H2O  or  alcohol  with  decomp. 
(Nickles,  C,  R.  60.  800.) 

Boron  phosphorus  bromide,  BBr3,  PBr3. 

Decomp.  by  H2O. 

Sol.  in  CS2,  and  CHC13.  Decomp.  by  al- 
cohol, ether,  etc.  (Tarible,  C.  R.  116.  1521.) 

BBr3,  PBr6.  SI.  sol.  in  cold,  easily  in  hot 
CS2.  (Tarible.) 

Boron  bromide  ammonia,  BBr3,  4NHa. 

Decomp.  by  H2O  and  alkalies.  (Besson,  C. 
R.  114.  542.) 

Boron  bromide  phosphine,  BBr3,  PH3. 

Violently  decomp.  by  H2O.  (Besson,  C.  R. 
113.  78.) 


110 


BORON  BROMIDE  PHOSPHORUS  CHLORIDE 


Boron  bromide  phosphorus  trichloride, 

2BBr3,PCl3. 

Decomp.  by  H2O.  Sol.  in  BBr3,  PC13,  CS2, 
and  CHC13.  Insol.  in  petroleum  ether. 
(Tarible,  C.  R.  1901,  132.  84.) 

Boron    bromide     phosphorus    pewtachloride, 

2BBr3,PCl5. 

Sol.  in  BBr3  and  CS2;  decomp.  by  H2O; 
insol.  in  light  petroleum.  (Tarible,  C.  R. 
1901,  132.  85.) 

Boron  bromide  phosphorus  dnodide,  2BBr3, 

P2I4. 

Sol.  in  BBr3,  CS2,  CHC13;  insol.  in  light 
petroleum;  decomp.  by  H2O.  (Tarible,  C.  R. 
1901,  132.  205.) 

Boron   bromide   phosphoryl   chloride,   BBr3, 

POC13. 

Very  easily  decomp.  (Oddo  and  Tealdi, 
Gazz.  ch.  it.  1903,  33.  (2)  431.) 

Boron  bromoiodide,  BBr2I. 

Decomp.  violently  by  H2O.  (Besson,  C.  R. 
112.  100.) 

BBrI2.    (Besson,  C.  R.  112.  100.) 

Boron  bromosulphide,  B2S3,BBr3. 

Decomp.  by  H2O.  (Stock,  B.  1901,  34. 
3040.) 

Boron  carbide,  B6C. 

Very  stable;  insol.  in  HF  and  in  HNO3; 
sol.  in  KOH  at  red  heat.  (Moissan,  Bull. 
Soc.  1894,  (3)  11.  1101.) 

Insol.  in  acids;  sol.  in  fused  alkali.  (Mois- 
san, C.  R.  1894,  118.  559.) 

BC  or  B2C2.  Insol.  in  all  the  usual  solvents. 
(Miillhauser,  Z.  anorg.  5.  92.) 

Boron  /n'chloride,  BC13. 

Rapidly  absorbed  by  H2O  and  alcohol  with 
decomposition. 

Boron  nitrosyl  chloride,  BC13,  NOC1. 

Decomp.  violently  by  H2O.  (Geuther,  J. 
pr.  (2)  8.  854.) 

Boron  phosphoryl  chloride,  BC13,  POC13. 

Decomp.  immediately  by  H2O.  (Gustav- 
son,  Zeit.  Chem.  1870.  521.) 

Boron  chloride  ammonia,  2BC13,  3NH3. 
Decomp.   by  H2O.      (Berzelius,   Pogg.   2. 

Boron  chloride  phosphine,  BC13,  PH3. 

Decomp.  by  H2O.  (Besson,  C.  R.  110. 
516.) 

Boron  chlorosulphide,  B2S3,BC13. 

Decomp.  by  H2O.  (Stock,  B.  1901,  34. 
3040.) 

Boron  ^'fluoride,  BF3. 

H2O  absorbs  700  vols.  BF3  gas  to  form  a 


liquid  of  1 .77  sp.  gr.  On  boiling,  Vs  of  the  BF3 
is  given  off,  and  a  residue  boiling  at  165-200°, 
with  composition  BF3+2H2O  or  HBO2  + 
3HF,  is  left.  (J.  Davy,  A.  ch.  86.  178.) 

1  ccm.  H2O  absorbs  at  0°  and  762  mm.  pres- 
sure 1.057  ccm.  BF3. 

1  vol.  cone.  H2SO4  of  1.85  sp.  gr.  absorbs 
50  vols.  BF3. 

Absorbed  by  alcohol  with  decomp. 

Cold  oil  of  turpentine  absorbs  6.8%  of 
BF3. 

Boron    fluoride    ammonia,    BF3,NH3,    BF3, 

2NH3,  and  BF3,  3NH3. 
Decomp.  by  H2O. 

Boron  fluoride  cyanhydric  acid,  BF3,  HCN. 
Very  unstable.     (Patein,  C.  R.  113.  85.) 

Boron  fluoride  phosphine,  2BF3,  PH3. 

Very  unstable  at  ordinary  temp.  Decomp. 
by  H2O.  (Besson,  C.  R.  110.  80.) 

Boron  hydride,  BH3. 

Not  obtained  free  from  H.  SI.  sol.  in  H2O. 
(Jones,  Chem.  Soc.  35.  41.)- 

See  Cyclofn'borene. 

B4H10.    B.-pt.  16-17°  at  760  mm. 

Very  unstable.  Takes  fire  spontaneously 
in  the  air. 

Decomp.  by  H2O,  dil.  HC1,  and  oxidized 
by  cone.  HNO3  with  explosive  violence. 

Absorbed  by  NaOH+Aq. 

Decomp.  by  alcohol.  Sol.  in  dry  benzene. 
(Stock,  B.  1912,  45.  3562.) 

B6Hi2.  B.-pt.  100°  at  atmospheric  pressure. 
Decomp.  by  H2O.  With  aqueous  alkalies, 
hydrogen  is  evolved.  (Stock,  B.  1912,  45. 

B8H.  Insol.  in  HC1.  Sol.  in  aqua  regia  and 
Br2+Aq.  (Winkler,  B.  1890,  23.  778.) 

B10Hi4.  M.-pt.  99.5°;  not  attacked  by  cold 
or  boiling  H2O.  Sol.  in  dil.  NaOH+Aq. 
Sol.  in  alcohol,  ether,  benzene,  and  CS2. 
(Stock,  B.  1913,  46.  3360.) 

Boron  iodide,  BI3. 

Very  hygroscopic,  and  instantly  decomp. 
by  H2O  or  alcohol.  Very  sol.  in  CS2,  CC14. 
C6H6;  less  sol.  in  PC13,  AsCl3,  and  a  great 
many  organic  liquids.  (Moissan,  C.  R.  112. 
717.) 

Boron  iodide  ammonia,  BI3,  5NH3. 

Decomp.  by  H2O.     (Besson,   C.   R.   114. 

542.) 

Boron  iodophosphide,  BI2P. 

Very  hygroscopic;  decomp.  by  H2O.  Not 
attacked  by  cold  cone.  H2SO4,  even  if  fuming, 
but  on  heating  decomposition  takes  place. 
Very  si.  sol.  in  CS2.  Insol.  in  benzene,  PC13> 
or  CC14.  (Moissan,  C.  R.  113.  624.) 

BIP.  Less  hygroscopic  than  BI2P,  but 
otherwise  the  properties  are  similar.  (Mois- 
san.) 


BOROTUNGSTATE,  AMMONIUM 


111 


Boron  nitride,  BN. 

Insol.  in.  H2O,  cone.  HNO3,  cone.  HC1  + 
Aq,  or  cone,  solutions  of  alkalies. 

Decomp.  by  hot  cone..  H2SO4  or  HF. 
(Wohler,  A.  74.  70.) 

Boron  /n'oxide,  B2O3. 

Deliquescent.  Sol.  in  H2O  with  a  large  in- 
crease in  temp.  (Ditte,  C.  R.  85.  1069.) 

1  pt.  dissolves — 

at    18.75°  in  47.01  pts.  H2O. 
27.75 
18.73 
15.13 
9.29 
7.28 
5.58 
4.74 


'    25° 
"    37.5 
"    50° 
"    62.5 

«    75° 
"    87.5 
"  100° 
Or  100  pts.  H2O  dissolve — 

at    18.75°     2.13  pts.  B2O3. 

"    25°          3.60 

"    37.5°      4.24 

"    50°          6.61 

"    62.5°     10.76 

"    75°        13.73 

"    87.5°     17.92 

"  100°        21.09 
(Brandes  and  Firnhaber,  Arch.  Pharm.  7.  50.) 

1  litre  H2O  dissolves — 

at      0°     ll.OOg.  B2O3. 
12°     16.50 " 
20°    22.49' 
40°     39.50' 
62°     64.50' 
80°     95.00' 
102°  164.50' 
(Ditte,  C.  R.  85.  1069.) 

Sat.  H2O  solution  boils  at  100°.  (Brandes 
and  Firnhaber.) 

Sat.  H2O  solution  boils  at  103.3°.  (Grif- 
fiths, Quar.  J.  Sci.  18.  90.) 

Sol.  in  acetic  acid,  hot  cone.  HCl+Aq, 
HNO3,  and  H2SO4.  From  the  three  latter  it 
separates  on  cooling  or  dilution  with  H2O. 

Solubility  in  Na2O+Aq  at  30. 

See  Borates,  sodium. 

Solubility  in  K2O+Aq  at  30°. 

See  Borates,  potassium. 

Insol.  in  hot  glacial  acetic  acid.  (Holt, 
Chem.  Soc.  1911,  100.  (2)  720.) 

Insol.  in  alcohol.     (Graham.) 

Sol.  in  alcohol.    (Berzelius,  Ebelmen.) 

Sol.  in  oils. 

See  also  Boric  acid. 

Boron  dioxide  potassium  fluoride,  B2O3,  2KF. 
Gradually  sol.  in  H2O.    Decomp.  by  much 
H2O.     Insol.  in  alcohol.     (Schiff  and  Sestini, 
A.  228.  82.) 

Boron  oxychloride,  BOC1. 

(Gustavson,  Zeit.  Chem.  1870.  521.) 
BOC13.    Slowly  decomp.  by  H2O.     (Coun- 

cler,  J.  pr.  (2)  18.  399.) 


Oxychlorides  of  either  the  above  formulae 
do  not  exist;  the  true  formula  for  boron  oxy- 
chloride is  B8OUC12.  (Lorenz,  A.  247.  226.) 

Boron  phosphide,  BP. 

Insol.  in  H2O.  Sol.  in  cone,  boiling  alkalies 
+Aq  with  decomp.  Decomp.  by  HNO3+Aq. 
(Besson,  C.  R.  113.  78.) 

Insol.  in  PC13,  AsCl3,  SbCl3,  CC14,  and  in 
fact  in  all  known  solvents. 

Not  attacked  by  boiling  H2O,  cone.  HC1,  or 
Hl-f  Aq.  Sol.  in  cone.  HNO3  with  decomp. 
on  heating.  Not  attacked  by  cold  H2SO4. 
(Moissan,  C.  R.  113.  726.) 

B5P3.  Not  attacked  by  boiling  cone.  HNO3 
+Aq.  Insol.  in  all  solvents.  (Moissan.) 

Boron  phosphoiodide. 
See  Boron  iodophosphide. 

Boron  selenide,  B2Se3. 

Violently  decomp.  by  H2O.  (Sabatier,  C. 
R.  112.  1000.) 

Boron  bisulphide,  B2S3. 

Decomp.  with  violence  with  H2O.  Com- 
bines with  alcohol  and  ether.  (Fremy,  A.  ch. 
(3)  38.  312.) 

Insol.  in  most  solvents,  but  si.  sol.  in  PC13 
without  decomp.;  more  sol.  in  SC12,  but  does 
not  crystallize  from  the  solution.  (Moissan, 
C.  R.  115.  203.) 

Boron  Jn'sulphide  ammonia,  B2S3,6NH3. 
Ppt.    (Stock,  B.  1901,  34.  3042.) 

Boron  pentasulphide,  B2S5. 

Decomp.  by  H2O  and  alcohol.  (Moissan, 
C.  R.  115.  271.) 

Borosulphuric  acid,  BOHSO4+SO3. 

Decomp.  by  H2O.  (Schultz-Sellac,  B.  4. 
12.) 

B(HSO4)3.  Very  deliquescent.  Easily  sol. 
in  fuming  H2SO4.  (D'Arcy,  Chem.  Soc.  55. 
155.) 

SO2(O.BO)2.  Hydroscopic.  Deliquescent. 
Sol.  in  H2O  with  decomp.  Decomp.  by  cold 
alcohols.  (Pictet,  Bull.  Soc.  1908,  (4)  3.  1121.) 

(SO3)2B2O3.  Hydroscopic.  Deliquescent. 
Sol.  in  H2O  with  decomp.  Decomp.  by  cold 
alcohols.  (Pictet,  Bull.  Soc.  1908,  (4)  3. 1121.) 

Borononotungstic      acid,      H4B2W9O32  + 

22H2O=9WO3,  B2O3,  2H2O+22H2O. 
Sol.  in  less  than  1/9  pt.  H2O,  and  as  easily 
sol.  in  alcohol  and  ether.    Sp.  gr.  of  aqueous 
solution  is  somewhat  under  3.    (Klein,  A.  ch. 
(5)  28.  370.) 

Aluminum  borononotungstate,  A14(B2W9O32)3 

+65H2O. 
Extremely  sol.  in  H2O.    (Klein.) 

Ammonium ,  (NH4)4B2W9O32  +  18H2O. 

Quickly  effloresces.    (Klein.) 


112 


BOROTUNGSTATE,  BARIUM 


Barium     borowo;zotungstate,     Ba2 

19H2O.       • 
Sol.  in  4  pts.  cold,  and  less  than  Y<>  pt.  hot 
H20.    (Klein.) 

Cadmium ,  Cd2B2W9O32  +  18H2O. 

Deliquescent. 

100  pts.  of  salt  dissolve  in  less  than  8  pts. 
H2O  at  19°.  Sp.  gr.  of  solution  is  3.28. 
(Klein.) 

Sp.  gr.  of  sat.  solution  at  15.6°/4°  =  3.2887; 
at  16.2°/4°=  3.2868.  (Kahlbaum,  Z.  anorg. 
1902,  29.  229.) 

Calcium ,  Ca2B2W9O32+15H2O. 

Sol.  in  Vio  pt.  H2O.  Solution  has  sp.  gr.  = 
3.10.  (Klein.) 

Cerium ,  Ce4(B2W9O32)3+57H2O. 

Very  sol.  in  H2O;  sp.  gr.  of  solution  is  over  3. 

Chromium ,  Cr4(B2W9O32)3+74H2O. 

Very  sol.  in  H2O;  sp.  gr.  of  solution  is  2.80. 
(Klein.) 

Cobalt ,  Co2B2W9O32  +  18H2O. 

Very  sol.  in  H2O;  sp.  gr.  of  solution  sat.  at 
19°  =  3.36.  (Klein.) 

100  pts.  H2O  dissolve  306.8  pts.  anhydrous 
salt  at  16.2°;  288  pts.  at  18.5°;  299.7  pts.  at 
19.6°;  286  pts.  at  21.8°. 

Sp.  gr.  of  solution  sat.  at  19.2°/4°  =  3.1369. 
(Kahlbaum,  Z.  anorg.  1902,  29.  218.) 

Copper ,  Cu2B2W9O32  +  19H2O. 

25  pts.  H2O  dissolve  100  pts.  salt.  Sp.  gr. 
of  solution  =  2. 6.  (Klein.) 

Lead ,  Pb2B2W9O32+llH2O. 

SI.  sol.  in  cold,  easily  sol.  in  hot  H2O. 
(Klein.) 

Lithium ,  (?). 

Very  sol.  in  H2O.  Sp.  gr.  of  solution  is 
about  3. 

Magnesium ,  Mg2B2W9O32+22H2O. 

Very  sol.  in  H2O.    (Klein.) 

Manganous ,  Mn2B2W9O32  +  17H20. 

100  pts.  dissolve  in  13  pts.  H2O.  Sp.  gr.  of 
solution  at  19°  =  3. 15.  (Klein.) 

Mercurous  — ,  3Hg2O,  B2O3,  9WO3  + 
14H2O  (?).  ...•"' 

Precipitate. 

Insol.  in  H2O.    (Klein.) 

Sol.  in  20,000  pts.  dil.  cold,  and  1000  pts 
boiling  HNO3+Aq  of  1.42  sp.  gr. 

Nickel ,  Ni2B2W9O32  +  18H2O. 

Very  sol.  in  H2O;  sp.  gr.  of  sat.  solution  at 
19°  =  3.32. 


100  pts.  H2O  dissolve  261.6  pts.  at  21.2°. 
Sp.     gr.     15.75°/4°     of    solution  =2.295 
(Kahlbaum,  Z.  anorg.  1902,  29.  218.) 


Potassium  boronorcotungstate,  K4B>W9O3>  + 

13H2O. 

5  pts.  salt  dissolve  in  8  pts.  H2O  at  19°  to 
form  a  solution  of  1.38  sp.  gr.  The  solution 
sat.  at  100°  has  sp.  gr.  of  over  2.  (Klein.) 

Silver ,  Ag4B2W9O32  +  14H2O. 

Very  si.  sol.  in  H2O. 
Sodium ,  Na2H2B2W9O32+23H2O. 

Very  sol.  in  H2O.  Solution  sat.  at  19°  con- 
tains 84  pts.  salt  to  16  pts.  H2O.  (Klein.) 

Na4B2W9O32  +  12H2O.  Sol.  in  less  than  l/3 
pt.  H2O. 

Thallium ,  T12B2W9O32+5H2O. 

SI.  sol.  in  hot  H2O  and  nearly  insol.  in  cold 
H2O.  (Klein.) 

Uranyl •,  (UO3)3(B2W9O30)2+30H2O. 

Very  sol.  in  H2O.    (Klein.) 
Sp.  gr.  of  solution  =  3.1. 

Zinc ,  Zn2B2W9O32+2H2O. 

Very  sol.  in  H2O.  Sp.  gr.  of  solution  =3.15. 
(Klein.) 

Borodecitungstic  acid. 

Barium     borodecitungstate,     Ba2B2Wi0O35  + 
20H2O.  M> 

Sol.  in  H2O.    (Klein,  C.  R.  99.  35.) 

Boroduodecitungstic  acid,  H8B2Wi2O43  = 

4H2O,  B2O3,  12  WO3. 

Known  only  in  solution,  which  decomposes 
into  borommotungstic  acid  and  tungstic  acid, 
when  evaporated  to  a  certain  concentration. 
(Klein,  C.  R.  99.  35.) 

Barium  potassium  borodwodea'tungstate, 
3BaO,  K2O,  B2O3,  12WO3+28H2O. 

Potassium ,  K8B2Wi2O43+21H2O. 

Sol.  in  H2O.    (Klein.) 

2K20,  12WO3,  B2O3  +  18H2O.  Sol.  in  H2O. 
(Klein.) 

RoToquatuordecitungstic  acid,  HioBoWi4O5i 

=  6H2O,  B2O3,  14WO3. 
Has  not  been  obtained  in  the  free  state. 
(Klein,  A.  ch.  (5)  28.  353.) 

Barium  TooToquatuordecitungstate, 

Ba3B2W14O48  =  3BaO,     B2O3,     14W03  + 
5H20. 

•  SI.  sol.  in  H2O.    (Klein.) 

arium    sodium    ,    S^BaO, 

5H2O,  B2O3,  14WO3+29H2O. 

Potassium ,  3K2O,  H2O,  B2O3,  14WO3- 

22H2O. 

Sol.  inH2O.    (Klein.) 
Silver ,  Ag6H2B2W14O49+7H2O. 

Nearly  insol.  in  cold  H2O.    (Klein.) 
Sodium ,  Na4H8B2W14O51+29HoO. 

Sol.  in  H2O     (Klein.) 


BROMAURATE,  MANGANESE 


113 


Sodium   strontium  boToquatttordecitungstaie, 
3HSrO,  l^Na2O,  B2O3, 14WO3+29H2O. 
Decomp.  by  H2O.    (Klein.) 

BoTOundevigintitungstic  acid. 

Barium    boroundevigintitungstate,    4BaO, 

B2O3,  19WO3+30H2O. 
Can   be   cryst.   from   H2O.      (Ebenhusen, 
Dissert.  1905.) 

BoToquattuoretvigintitungstic    acid,    B2O3, 

24WO3+66H2O. 

Deliquescent.  Somewhat  more  sol.  in  H2O 
than  B2O3,  28WO3+62H2O.  Also  more 
stable.  (Copaux,  C.  R.  1908,  147.  975.) 

Barium    boToquattuoretrigintitungsta.te, 
5BaO,  B2O3,  24WO3+54H2O. 

100  pts.  H2O  dissolve  50  pts.  salt.  (Copaux, 
A.  ch.  1909,  (8)  17.  217.) 

6BaO,  B2O3,  24WO3+58H2O.  (Copaux, 
I.e.) 

Cadmium    ,     5CdO,     B2O3,     24WO3  + 

51H2O. 
Extremely  sol.  in  H2O.    (Copaux,  I.  c.) 

Calcium ,  5CaO,  B2O3,  24WO3+44H2O. 

Very  sol.  in  H2O.    (Copaux,  I.  c.) 

Lithium ,  15Li2O,  B2O3,  24WO3+38H2O. 

(Copaux,  /.  c.) 

Magnesium   — 
42H2O. 


5MgO,    B2O3,    24WO3  + 


Very  sol.  in  H2O.     (Copaux,  I.  c.) 


9Hg2O,    B2O3,    24WO3  + 


5K2O,     B2O3,     24WO3 


Mercurous    

25H.O. 

(Copaux,  I.  c.) 

Potassium  

36H2O. 

(Copaux,  I.  c.) 
Sodium ,  5Na2O,  B2O3,  24WO3+5H2O. 

As  NH4  salt.    (Copaux,  /.  c.) 

BoToquinquetvigintitungstic  acid. 

Potassium    boroquinquetvigintitungstate, 

5K2O,  B2O3, 25WO3+34H2O.    (Ebenhusen, 
Dissert.  1905.) 

Boroduodetrigintatungstic  acid,  B2O3, 

28WO3+62H2O. 

Decomp.  in  boiling  aqueous  solution.    (Co- 
paux, C.  R.  1908,  147.  975.) 

Potassium  boTodiiodetrigintatungstate,  6K2O, 

B2O3,  28WO3+42H2O. 
Decomp.    by   boiling    alkalies.      (Copaux, 
A.  ch.  1909  (8)  17.  217.) 

Borovanadic  acid. 

Sol.  in  H2O.     Easily  decomp.     (Guyard, 
Bull.  Soc.  (2)  25.  354.) 


Afetabromantimonic  acid,  HSbBr6+3H2O. 

Very  hydroscopic.  Loses  Br2  in  the  air. 
Decomp.  by  H2O  with  separation  of  anti- 
monic  acid.  (Weinland,  B.  1903,  36.  256.) 

Ammonium  metobromantimonate, 

NH4SbBr6+H2O. 

Loses  Br2  in  the  air.  Decomp.  by  H2O. 
(Weinland,  I.  c.)  - 

Iron  (ferric)  wdabromantimonate, 

Fe(SbBr6)3  +  14H2O. 

Very  hydroscopic.  Decomp.  by  H2O. 
(Weinland",  I.  c.) 

Lithium      wetabromantimonate,     LiSbBre  + 

4H2O. 

Very  hydroscopic.  Loses  Br2  in  the  air, 
Decomp.  by  H2O.  (Weinland,  L  c.) 

Nickel    metobromantimonate,    Ni(SbBr6)2  + 

12H2O. 

Hydroscopic.  Decomp.  by  H2O.  (Wein- 
land, I.  c.)  ^ 

Potassium    /^etobromantimonate,    KSbBre-h 

H2O. 

Loses  Br2  in  the  air.  Decomp.  by  H2O. 
(Weinland,  I.  c.) 

Bromarsenious  acid. 

See  Arsenyl  bromide. 
Bromauric  acid,  HAuBr4+3H2O. 

(Lengfeld,  Am.  Ch.  J.  1901,  26.  329.) 

+5H2O.  Very  sol.  in  H2O.  (Thomsen,  J. 
pr.  (2)  13.  337.) 

-f  6H2O.    Sol.  in  ether  and  CHC13  without 
decomp.     (Lengfeld,  Am.  Ch.  J.   1901,  26. 
329.) 
Ammonium  bromaurate,  NH4AuBr4. 

Ppt.    (Gutbier,  Z.  anorg.  1914,  85.  358.) 

Barium  bromaurate. 

Not  deliquescent.    Sol.  in  H2O.    (v.  Bons- 
dorff,  Pogg.  17.261.) 
Caesium  bromaurate,  CsAuBr4. 

SI.  sol.  in  H2O  or  alcohol.  Insol.  in  ether. 
(Wells  and  Wheeler,  Sill.  Am.  J.  144.  157.) 

Ppt.    (Gutbier,  Z.  anorg.  1914,  85.  360.) 

Cerium  bromaurate,  CeAuBr6+8H2O. 

Sol.  in  H2O.    ( Jolin,  Bull.  Soc.  (2)  21.  533.) 

Didymium  bromaurate,  DiAuBr6-f-9H20. 
Very  deliquescent.    Sol.  in  H2O.    (Cleve.) 

Lanthanum  bromaurate,  LaAuBr6+9H2O. 

Sol.  in  H2O.    (Cleve.) 
Magnesium  bromaurate. 

Deliquescent  in  moist  air.  (v.  Bonsdorff.) 
Manganese  bromaurate. 

Deliquescent,    (v.  Bonsdorff.) 


114 


BROMAURATE,  POTASSIUM 


Potassium  bromaurate,  KAuBr4. 

SI.  sol.  in  H2O.  More  sol.  in  cold  alcohol 
than  in  H2O.  (v.  Bonsdorff.) 

+2H2O.  Sol.  in  5.12  pts.  H2O  at  15°,  1.56 
pts.  at  40°,  and  0.48  pt.  at  67°.  Decomp.  by 
ether.  SI.  sol.  in  KBr+Aq.  (Schottlander, 
A.  217.  314.) 

+5H2(X    Efflorescent,     (v.  Bonsdorff.) 

Rubidium  bromaurate,  RbAuBr4. 
As  caesium  bromaurate. 
Ppt.    (Gutbier,  Z.  anorg.  1914,  85.  359.) 

Samarium  bromaurate,  SmAuBr6+10H2O. 

Very  deliquescent.  (Cleve,  Bull.  Soc.  (2) 
43.  165.) 

Sodium  bromaurate,  NaAuBr4. 

Slowly  sol.  in  H2O.    (v.  Bonsdorff.) 
Zinc  bromaurate,  Zn(AuBr4)2. 

Very  deliquescent,    (v.  Bonsdorff.) 

Bromauricyanhdric  acid. 

Not  known  in  free  state.     * 

Barium  bromauricyanide,  Ba[Au(CN)2Br2]2  + 

10H20. 

Very  sol.  in  hot  or  cold  H2O,  also  in  alcohol. 
(Lindbom,  Lund.  Univ.  Arsk.  12.  No.  6.) 

Cadmium  bromauricyanide,  Cd[Au(CN)2Br2]2 

+6H20. 

Very  sol.  in  hot  or  cold  H2O,  but  solution  is 
unstable.  (Lindbom.) 

Calcium  bromauricyanide,  Ca[Au(CN)2Br2]2 
+  10H20. 

Extremely  sol.  in  H2O  and  alcohol.  (Lind- 
bom.) 

Cobalt  bromauricyanide,  Co[Au(CN)2Br2]2  + 

9H20. 

Moderately  sol.  in  H2O.  Less  sol.  than 
other  bromauricyanides.  (Lindbom.) 

Potassium   bromauricyanide,    KAu(CN)2Br 

+3H2O. 
Sol.  in  H2O  and  alcohol. 

Sodium  bromauricyanide,  NaAu(CN)2Br2  + 

2H2O. 
Very  sol.  in  H2O  or  alcohol.     ;IJ* 

Strontium  bromauricyanide,  Sr[Au(CN)2Br2 

+zH20. 
Very  sol.  in  H2O  or  alcohol. 

Zinc    bromauricyanide,    Zn[Au(CN)2Br2]2  + 

8H2O. 
Easily  sol.  in  cold  or  hot  H2O. 

Bfomhydric  acid,  HBr. 

Very  sol.  in  H2O. 

The  most  concentrated  HBr+Aq  has  a  sp. 
gr.  of  1.78,  and  contains  82.02%  HBr.  (Cham- 
pion and  Pellat,  C.  R.  70.  620.)  This,  or  a 
weak  acid  on  heating  leaves  a  residue,  which 


t° 

Pts. 
HBr 

t° 

Pts. 
HBr 

t° 

Pts. 
HBr 

—25 
—20 
—15 
—10 

2.550 
2.473 
2.390 
2.335 

—5 
0 
+  10 

+25 

2.280 
2.212 
2.103 
1.930 

+50 

+75 
+  100 

1  .  715 

1.505 
1.300 

distils  unchanged  at  125-125.5°  under  785 
mm.  pressure,  and  contains  48.17%  HBr 
(Topsoe);  at  126°  under  758  mm.  pressure, 
and  contains  46.83%  HBr  (Bineau);  and  has 
sp.  gr.  =  1.486  at  20°  (Bineau);  sp.  gr.  =  1.48  at 
20°  (Champion  and  Pellat);  sp.  gr.  =  1.49  at 
20°  (Topsoe)! 

According  to  Roscoe  (A.  116.  214)  an  acid 
of  constant  composition,  obtained  by  boiling 
a  stronger  or  a  weaker  acid,  if  distilled  under 
752-762  mm.  pressure,  contains  47.38-47.86% 
HBr,  and  boils  at  126°  at  760  mm.  pressure; 
but  the  composition  is  dependent  on  the 
pressure,  as,  for  example,  under  1952  mm. 
pressure,  the  residue  boils  at  153°,  and  con- 
tains 46.3%  HBr.  (Roscoe.) 

By  conducting  dry  air  through  HBr+Aq 
an  acid  is  obtained  containing  51.65%  HBr  if 
at  16°,  and  49.35%  HBr  if  at  100°  (Roscoe). 

1  vol.  H2O  dissolves  600±vols.  HBr  at  10°. 
(Berthelot,  C.  R.  76.  679.) 

1  pt.  H2O  at  t°  and  760  mm.  pressure 
dissolves  pts.  HBr. 


(Roozeboom,  R.  t.  c.  4.  107.) 

Absorption  by  1  pt.  H2O  at  t°  and  p  pressure 
in  mm. 

t°=  —25°. 


P 

Pts.  HBr 

P 

Pts.  HBr 

760 
300 
140 

2.550 
2.263 
2.120 

100 
1 
0.5 

2.056 
1.755 
1.10 

t°=—  20°. 

p 

Pts.  HBr 

P 

Pts.  HBr 

760 
375 

180 

2.473 
2  267 
2.119 

130 
20 

2.056 
1.850 

t°=  —15°, 

P 

Pts.  HBr 

p 

Pts.  HBr 

760 
470 
250 

2.390 
2.266 
2.119 

175 
102 

2.056 
1.980 

t°=—  11.3°. 

p 

Pts.  HBr 

P 

Pts.  HBr 

760 
570 

2.350 
2.265 

310 
216 

2.118 

2.055 

BROMATE,  ALUMINUM 


115 


t°=  —5°. 

Sp.  gr. 

of  HBr+Aq  at  15°. 

p 

Pts.  HBr 

p 

Pts   HBr 

°7 

°7 

c/ 

HBr 

Sp.  gr. 

HBr 

Sp.  gr. 

HBr 

Sp.  gr. 

760 

2.280 

430 

2.117 

n.  J5r 

730 

2.264 

298 

2.055 

1 

1.0082 

18 

1.145- 

35 

1.314 

0 

1  m  ^^ 

1  Q 

1      1  ^4. 

OR 

1      *^9A 

t°  =  0°. 

4fi 

3 

1^0230 

20 

M63 

OvJ 

37 

1.338 

4 

1  0305 

21 

1.172 

38 

1.350 

P 

Pts.  HBr 

p 

Pts.  HBr 

5 

22 

M81 

39 

1^362 

Io^rcr 

760 

2.212 

380 

2.054 

6 

7 

1  .046 
1.053 

23 
24 

1  .  190 
1.200 

40 
41 

.375 

1.388 

540 

2.116 

5 

1.085 

8 

1.061 

25 

1.209 

42 

1.401 

(Roozeboom,  R.  t.  c.  4.  107.) 

9 
10 

1.069 
1.077 

26 

27 

1.219 
1.229 

43 
44 

1.415 
1.429 

Sp.  gr.  of  HBr+Aq. 

11 

1.085 

28 

1.239 

45 

1.444 

12 

1  .093 

OQ 

i    24Q 

46 

1  .459 

Sp.  gr. 

%  HBr 

Temp. 

Sp.  gr. 

%  HBr 

Temp. 

13 

l'l02 

30 

-L  .  ^Tti7 

1.260 

47 

1^474 

1.055 

7.67 

14° 

1.335 

36.67 

13° 

14 
15 

1.110 
1.119 

31 

32 

1.270 
1.281 

48 
49 

1.490 
1.496 

1.075 

10.19 

14° 

1.349 

37.86 

13° 

16 

1.127 

33 

1.292 

50 

1.513 

1.089 

11.94 

14° 

1.368 

39.13 

13° 

17 

1.136 

34 

1.303 

1  097 

1 

2  96 

14° 

1  419 

;  12 

13° 

1.118 

15^37 

14° 

1.431 

43.99 

13° 

(Biel 

,  C.  C.  1882.  148.) 

1.131 

1 

6  92 

14° 

1  438 

44 

L  62 

13° 

1.164 

20^65 

14° 

1.451 

45.45 

14° 

Absorbed   by 

alcohol   with  .formation   of 

1.200 
1.232 
1.253 
1.302 

24.35 
27.62 
29.68 
33  84 

13° 
13° 

13° 
13° 

1.460 
1.485 
1.490 

46.09 

47.87 
48.17 

13° 
14° 

14° 

C2H5Br. 
The  composition  of  the  hydrates  formed  by 
HBr  at  different  dilutions  is  calculated  from 
determinations  of  the  lowering  of  the  fr.  pt. 

T3rOQU. 

r>orl     ITIT-     T^ 

Rr     Q 

nrl     r»f    fVi 

p    (\c\rtf 

iint.ivit.v 

(Topsoe,  B.  3.  404.) 

and  sp.  gr.  of  HBr+Aq.    (Jones,  Am.  Ch.  J. 

1905, 

3d    39.fi  1 

Sp.  gr.  of  HBr+Aq  at  14°. 

+H2O.    (Roozeboom,  R.  t. 

c.  5.  363.) 

%  HBr 

Sp.  gr. 

%HBr 

Sp.  gr. 

%HBr 

Sp.  gr. 

+2H2O.    (Berthelot,  A.  ch.  (5)  14.  369.) 
(Pickering  Chem.    Soc.1894,  64  (2)  232. 

1 

007 

18 

1.140 

35 

.314 

Mpt.    —11.2°.    (Pickering,  I.  c.) 

2 

.014 

19 

1.149 

36 

.326 

+3H2O.    Mpt.    —48.0°. 

(Pickering.) 

3 

.021 

20 

1.158 

37 

.338 

+4H2O.    Mpt.  —55.8°.     (Pickering.) 

4 

.028 

21 

1.167 

38 

.351 

+5H2O.    (Pickering.) 

5 
6 

.035 
.043 

22 
23 

1.176 
1.186 

39 
40 

.363 
.376 

Bromhydric 

cyanhydric 

acid, 

.  3HBr, 

7 

1 

.050 

24 

1.196 

41 

.389 

2HCN. 

8 

1 

.058 

25 

1.206 

42 

.403 

Decomp.  by  H2O  and  alcohol. 

9 

1 

.065 

26 

.215 

43 

.417 

Insol.  in  ether.     (Gautier, 

A.  ch 

(4)  17. 

10 

1 

.073 

27 

.225 

44 

.431 

141.) 

11 
12 
13 
14 
15 
16 
17 

1 

1 
1 
1 

1 

i 

i 

.081 
.089 
.097 
.106 
.114 
.122 
.131 

28 
29 
30 
31 
32 
33 
34 

.235 
.246 
.257 
.268 
.279 
1.290 
1.302 

45 
46 
47 

48 
49 

.445 
.459 
.473 

.487 
.502 

Bromic  acid,  HBrO3. 

Known  only  in  aqueous  solution. 
Solution  evaporated  on  water  bath  decom- 
poses when  it  contains  4.26%  HBrO3.     In 
vacuo,   an  acid   containing  50.59%   HBrO3 
corresponding  to  formula  HBrO3+7H2O  can 

be  ob 

hamed. 

(Topsoe, 

calculated  by  Gerlach, 

Z.  anal.  27. 

Not  decomp. 

by  dil.  HNO3, 

orH2SO4+Aq. 

316.) 
Sp.gr.  of  HBr+Aq  at  15°. 

Cone.  H2SO4  decomposes. 
Alcohol  and  ether  are  quickly  oxidized  by 
HBrO3. 

%  HBr 

Sp.  gr. 

%HBr 

Sp.  gr. 

%HBr 

Sp.  gr. 

Bromates. 

5 
10 
15 

1 

1 

1 

.038 
.077 
.177 

25 
30 
35 

1.204 
1.252 
1.305 

45 
50 

1.435 
1.515 

Most  of  the  bromates  are  very  sol 
a  few  are  si.  sol.,  but  none  are  insol., 
sol/being  AgBrO3  and  Hg2(BrO3)2. 

in  H2O, 
the  least 

20 

1 

.159 

40 

1.365 

Aluminum  bromate,  Al(BrO3)3. 

Only  i 

i  "moderate  degree  of  accuracy"  is 

Deliquescent. 

(Rammelsberg,    Pogg.    55. 

claimed 

242.) 

for  this  table.     (Wright,  C.  N.  23. 

63.) 
+9H2O.     Mpt.  62.3°.     Less  hygroscopic 

116 


BROMATE,  AMMONIUM 


than  A1(C1O3)2.    (Dobrosserdow,  C.  C.  1907. 
I,  1723.) 

Ammonium  bromate,  NH<BrO3. 

Decomposes  spontaneously;  sol.  in  H2O. 
(Rammelsberg,  Pogg.  62.  85.) 

Barium  bromate,  Ba(BrO3)2. 

Solubility  of  Ba(BrO3)2  in  H2O.  100  g.  sat. 
Ba(BrO3)2+Aq  at  t°  contain  g.  anhy- 
drous Ba(BrO3)2. 


Bismuth  bromate. 

Known  only  in  solution,  which  decomp.  on 
evaporation.    ( Rammelsberg,  Pogg.  55.  76.) 

Cadmium  bromate,  Cd(BrO3)2+H2O. 

Sol.  in  0.8  pt.  cold  H2O.     (Rammelsberg, 
Pogg.  55.  74.) 

+2H2O.    (Topsoe,  J.  B.  1872,  164.) 

bromate 


Grams 

t 

grains 
.Ba(BrOs)s 

t° 

Ba(BrOr-)2 

Eutectic  point 

—0.034°  ±0.002° 

0.280 

50° 

1.72 

0° 

0.286 

60° 

2.271 

+  10° 

0.439 

70° 

2.922 

20° 

0.652 

80° 

3.521 

25° 

0.788 

90° 

4.26 

30° 

0.95 

98.7° 

5.256 

40° 

1.31 

*99.65° 

5.39 

ammonia,    Cd(BrO3)2, 
(Rammelsberg,  Pogg. 


*  99.65°  is  bpt.  at  740  mm.  =  100.39°  at 
760mm. 

(Anschutz,  Z.  phys.  Ch.  1906,  56.  240.) 

100  g.  sat.  Ba(BrO3)2+Aq  contain  0.793  g. 
Ba(BrO3)2  at  25°.  Sp.  gr.  of  the  solution 
at  25°/4°  =  1.0038.  (Harkins  J.  Am.  Chem. 
Soc.  1911,  33.  1815.) 

Solubility  of  Ba(BrO3)2  in  salts+Aq  at  25°. 
C  =  concentration  of  salt  in  salt+Aq  in  milli- 

equivalents  per  1. 
di  =Sp.  gr.  at  2574°  of  salt+Aq. 
S=  solubility  of  Ba(BrO3)2  in  salt+Aq  ex- 
pressed in  milliequivalents  per  1. 
d2  =  sp.  gr.  at  2574°  of  Ba(BrO3)2+salt+Aq. 


Salt 

C 

d, 

s 

d2 

None 

40.18 

1.0038 

KN03 

25.018 
50.032 
99.970 

0.9985 
1.0030 
1.0033 

43.86 
47.03 
52.13 

1.0059 
1.0081 
1.0120 

Ba(NO?)2 

25.018 
50.039 
99.97 
199.95 

1.0003 
1.0025 
1.0073 
1.0183 

36.77 
34.74 
32.63 
30.95 

1  .  0059 
1.0083 
1.0132 
1.0233 

KBrO3 

24.988 
49.971 
99.85 

1.0001 
1.0031 
1.0093 

26.53 
17.37 

8.76 

1.0046 
1.0062 
1.0109 

Mg(N03)2 

100.0 

52.57 

1.0114 

(Harkins,  J.  Am.  Chem.  Soc.  1911,  33.  1815.) 

+H2O.  Sol.  in  130  pts.  cold,  and  24  pts. 
boiling  H2O.  (Rammelsberg,  Pogg.  52.  81  ) 

Decomp.  by  H2SO4,  or  HCl+Aq. 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 


Cadmium 
3NH3. 

Decomp.  by  H2O. 
55.  74.) 

Cd(BrO3)2,  4NH3.  Ppt.  (Ephraim,  B. 
1915,  48.  51.) 

Calcium  bromate,  Ca(BrO3)2+H2O. 

Sol.  in  1.1  pts.  cold  H2O.  (Rammelsberg, 
Pogg.  52.  98.) 

Cerous  bromate,  Ce(BrO3)3+9H20. 

Easily  sol.  in  H2O.  (Rammelsberg,  Pogg. 
55.  63.) 

Mpt.  49°;  very  sol.  in  H2O  with  decomp. 
(James,  J.  Am.  Chem.  Soc.  1909,  31.  914.) 

Cobaltous  bromate,  Co(BrO3)2+6H2O. 

Sol.  in  2.2  pts.  cold  H2O;  sol.  in  NH4OH 
+Aq.  (Rammelsberg,  Pogg.  55.  71.) 

Cupric  bromate,  basic,  6CuO,  Br2O5  +  10H2O. 
Ppt.    (Rammelsberg,  Pogg.  55.  78.) 

Cupric  bromate,  Cu(BrO3)2+6H2O. 

Easily  sol.  in  H2O.  (Rammelsberg,  Pogg. 
52.  92.) 

Cupric  bromate  ammonia,  Cu(BrO3)2,  4NH3. 

Completely  sol.  in  a  little  H2O,  but  de- 
comp. by  dilution. 

Insol.  in  alcohol.  (Rammelsberg,  Pogg.  52. 
92.) 

Didymium  bromate,  Di(BrO3)3+9H2O. 
Sol.  in  H2O.    (Marignac.) 

Dysprosium  bromate,  Dy(BrO3)3+9H2O. 

Mpt.  78°.  Easily  sol.  in  H2O.  Difficultly 
sol.  in  alcohol.  (Jantsch,  B.  1911,  44.  1275.) 

Erbium  bromate,  Er(BrO3)3+9H2O. 
Very  sol.  in  alcohol  and  H2O. 

Glucinum  bromate. 

Deliquescent. 

Iron  (ferrous)  bromate,  Fe(BrO3)2. 

Sol.   in  H2O,   but   solution  decomp.    very 


Iron  (ferric)  bromate,  5Fe2O3,  Br2O5+30H2O. 
Partially  sol.  in  H2O,  with  separation  of  a 
more  basic  salt.  Sol.  in  HBO3+Aq.  (Ram- 
melsberg, Pogg.  55.  68.) 

Lanthanum  bromate,  La(BrO3)3+9H2O. 

Sol.  in  3y2  pts.  H2O  at  15°.  (Marignac, 
Ann.  Min.  (5)  15.  274.) 

Mpt.  37.5°  in  its  water  of  crystallization. 
416  pts.  are  sol.  in  100  pts.  H2O  at  25°. 
(James,  J.  Am.  Chem.  Soc.  1909,  31.  913.) 


BROMATE,  POTASSIUM 


117 


Lead    bromate,    basic,    3PbO,    Pb(BrO3)2  + 

2H2O. 
Ppt.    (Stromholm,  Z.  anorg.  1904,  38.  441.) 

Lead  bromate,  Pb(BrO3)2. 

SI.  SDl.  in  H2O.  13.37  x  IQ-'g.  are  contained 
in  1  liter  of  sat.  solution  at  20°.  (Bottger, 
Z.  phys.  Ch.  1903,  46.  603.) 

+H2O.  Sol.  in  75  pts.  cold  H2O.  (Ram- 
melsberg,  Pogg.  52.  96.) 

Lithium  bromate,  LiBrO3. 

Very  deliquescent,  and  sol.  in  H2O.  (Ram- 
melsberg,  Pogg.  A.  55.  63.) 

Not  deliquescent.  (Politilitzin,  B.  23. 
545  R.) 

Sp.  gr.  of  solution  sat.  at  18°  =  1.833,  and 
contains  60.4%  LiBrO3.  (Mylius,  B.  1897, 
30.  1718.) 

+H2O.    Not  deliquescent.     (Potilitzin.) 

Magnesium  bromate,  Mg(BrO3)2+6H2O. 

Efflorescent.  Sol.  in  1.4  pts.  cold  H2O  at 
15°.  Melts  in  its  water  of  crystallization  when 
heated.  (Rammelsberg,  Pogg.  52.  89.) 

Mercurous  bromate,  basic,  2Hg2O,  Br2O5. 

Insol.  in  warm  H2O.  Sol.  in  HNO3+Aq. 
(Rammelsberg,  Pogg.  55.  79.) 

Mercurous  bromate,  Hg2(BrO3)2. 

Decomp.  by  H2O  into  basic  salt.  Difficultly 
sol.  in  HNO3+Aq;  easily  sol.  in  HCl+Aq. 
(Rammelsberg.) 

Mercuric  bromate,  basic,  2HgO,  Br2O5+H2O. 

Slowly  decomp.  by  cold,  quickly  by  hot 
H2O  into  oxide  and  an  acid  salt. 

Easily  sol.  in  dil.  acids.  (Topsoe,  W.  A.  B. 
66,  2.  2.) 

Mercuric  bromate,  HgBr03+2H2O. 

Sol.  in  650  pts.  cold,  and  64  pts.  boiling 
H2O.  SI.  sol.  in  HNO3+Aq.  Easily  sol.  in 
HCl+Aq.  (Rammelsberg,  Pogg.  55.  79.) 

Mercuric  bromate  ammonia. 

Sol.  with  decomp.  in  HCl+Aq.  (Storer's 
Diet.) 

Neodymium  bromate,  Nd(BrO3)3+9H2O. 

Mpt.  66.7°.  146  pts.  are  sol.  in  100  pts. 
H2O  at  25°.  (James,  J.  Am.  Chem.  Soc. 
1909,  31.  915.) 

Nickel  bromate,  Ni(BrO3)2+6H2O. 

Sol.  in  3.58  pts.  cold  H2O.  (Rammelsberg, 
Pogg.  55.  69.) 

Nickel  bromate  ammonia,  Ni(BrO3)2,  2NH3. 

Sol.  in  H2O,  with  decomposition  of  the 
major  portion.  Insol.  in  alcohol.  (Rammels- 
berg, I.  c.) 

Ni(BrO3)2,  6NH3.  Ppt.  (Ephraim,  B. 
1915,  48.  50.) 

Potassium  bromate,  KBrO3. 

100  pts.  H2O  dissolve  6.58  pts.  KBrO3  at 
15°  (Rammelsberg).  100  pts.  H2O  dissolve 
5.83  pts.  KBrO3  at  17.1°  (Pohl.  W.  A.  B.  6. 


%KBr03 
Sp.  gr.    . 

1 
1.009 

2 
1.016 

3 
1.024 

4 
1.031 

5 
1.039 

%KBr03 
Sp.gr.   . 

6 
1.046 

7 
1.054 

8 
1.062 

9 
1.070 

10 
1.079 

(Gerlach,  Z.  anal.  8.  290.) 
Solubility  of  KBrO3  in  salts  +Aq  at  25°. 

i 

Salt 

Moles  of  KBrO3  sol.  in  1  liter  of 

.5-N 
solution 

N 
solution 

2-N 
solution 

3-N 

solution 

4-N 

solution 

NaNO3 
NaCl 

9.5745 
3.5220 

3.6497 
3.5616 

0.7680 
0.6042 

0.9026 
0.6244 

1.031 
0.640 

595);  at  0°,  3.11  pts.;  at  20°,  6.92  pts.;  at  40°, 
13.24  pts.;  at  60°,  22.76  pts.;  at  80°,  33.90 pts. ; 
at  100°  49.75  pts.  KBrO3.  Sat.  solution  boils 
at  104°.  (Kremers,  Pogg.  97.  5.) 

1  1.  H2O  at  25°  dissolves  0.4715  moles 
KBrO3.  (Geffcken,  Z.  phys.  Ch.  1904,  49. 
296.) 

1-1.  H2O  dissolves  0.478  mol.  KBrO3  at  25°. 
(Rothmund,  Z.  phys.  Ch.  1909,  69.  539.) 

Sp.  gr.  of  KBrO3+Aq  at  19.5°. 


(Geffcken,  Z.  phys.  Ch.  1904,  49.  296.) 

Easily  sol.  in  liquid  HF.     (Franklin,   Z. 
anorg.  1905,  46.  2.) 

SI.  sol.  in  alcohol.    (Rammelsberg.) 
Insol.  in  absolute  alcohol. 

Solubility  in  organic  compds.+Aq  at  25°. 


Solvent 

Mol.  KBrOs  sol.  in 
1  litre 

Water 

0.478 

0.5-N  Methyl  alcohol 

0.444      • 

"      Ethyl  alcohol 

0.421 

"       Propyl  alcohol 

0.409 

'       Tert.  amyl  alcohol 

0.383 

'       Acetone 

0.425 

•       Ether 

0.395 

'       Formaldehyde 

0.397 

'      Glycol 

0.448 

'       Glycerine 

0.451 

'       Mannitol 

0.451 

'       Glucose 

0.463 

'       Sucrose 

0.431 

'      Urea 

0.477 

'       Dimethyl  pyrone 

0.478 

'       Ammonia 

0.445 

'       Diethylamine 
'       Pyridine 
'       Piperidine 

0.384 
0.415 
0.396 

'      Urethane 

0.433 

(       Formamide 

0.473 

'      Acetamide 

0.445 

'      GlycDcoll 

0.501 

'       Acetic  acid 

0.456 

"       Phenol 

0.426 

"       Methylal 

0.405 

"       Methyl  acetate 

0.420 

(Rothmund,  Z.  phys.  Ch.  1909,  69.  539.) 

118 


BROMATE,  PRASEODYMIUM 


Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B4  1904,  37.  4329.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,42.3790.) 

Praseodymium  bromate,  Pr(BrO3)3+9H2O. 

Mpt.  56.5°.  190  pts.  are  sol.  in  100  pts. 
H2O  at  25°.  (James,  J.  Am.  Chem.  Soc. 
1909,  31.  914.) 

Samarium  bromate,  Sm(BrO3)3+9H2O. 

Mpt.  75°.  114  pts.  are  sol.  in  100  pts.  H2O 
at  25°.  Very  si.  sol.  in  alcohol.  (James,  J. 
Am.  Chem.  Soc.  1909,  31.  915.) 

Scandium  bromate. 

(Crookes,  Roy.  Soc.  Proc.  1908,  80,  A,  518.) 
Silver  bromate,  AgBrO3. 

1  pt.  H2O  dissolves  0.00810 -pt.  AgBrO3  at 
24.5°.  (Noyes,  Z.  phys.  Ch.  6.  246.) 

Sol.  in  595.3  pts.  H2O  at  25°. 

Sol.  in  320.4  pts.  HNO3+Aq  (sp.  gr.  1.21) 
at  25°. 

Sol.  in  2.2  pts.  NH4OH+Aq  (sp.  gr.  0.96) 
at  25°.  (Longi,  Gazz.  ch.  it.  13.  87.) 

1  1.  H2O  dissolves  1.71  g.  AgBrO3  at  27°. 
(Whitby,  Z.  anorg.  1910,  67.  108.) 

SI.  sol.  in  H2O.  1.59  x  10-4  g.  are  con- 
tained in  1  liter  of  sat.  solution  at  20°. 
(Bottger,  Z.  phys.  Ch*.  1903,  46.  603.) 

Insol.  in  HNO3.  (Lowig.)  Easily  sol.  in 
NH4OH+Aq. 

Silver  bromate  ammonia,  AgBrO3,  2NH3. 

Decomp.  in  air  or  by  H2O.  (Rammels- 
berg,  Pogg.  52.  94.) 

Sodium  bromate,  NaBrO3. 

Sol.  in  2.7  pts.  H2O  at  15°.    (Rammelsberg.) 

100  pts.  H2O  dissolve  at— 

0°     20°     40°  60°     80°   100° 
27.54  34.48  50.25  62.5  75.75  90.9  pts.  NaBrO3. 
(Kremers,  Pogg.  94.  271.) 

Easily  forms  supersaturated  solutions. 

Sat.  solution  boils  at  109°.    (Kremers.) 

NaBrO3+Aq  containing  10.10%  NaBrO3 
has  sp.gr.  20°/20°  =  1.0818. 

NaBrO3+Aq  containing  11.09%  NaBrO3 
has  sp.  gr.  20°/20°  =  1.0900. 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896 
19.  278.) 

Sp.  gr.  of  NaBrO3-f  Aq  at  19.5°. 


%NaBr03    . 
Sp.gr.    .      . 

5 
1.041 

10 
1.083 

15 
1.129 

%NaBr03    . 
Sp.gr.    . 

20 
1.178 

25 
1.231 

30 
1.289 

(Kremers,  Pogg.  97.  5,  calculated  by  Gerlach, 
Z.  anal.  8.  290.) 

Moderately  sol.  in  liquid  NH3.    (Franklin 
Am.  Ch.  J.  1898,  20.  829.) 

Insol.  in  methyl  acetate.     (Naumann,  B. 

1909,  42.  3790.) 

Insol.   in   ethyl   acetate.      (Naumann,    B. 

1910,  43.  314.) 

Sodium  bromate  bromide,  3NaBrO3,  2NaBr 
+3H2O. 

Decomp.  by  H2O  or  alcohol.  (Fritzsche.) 
Strontium  bromate,  Sr(BrO3)2+H2O. 

Sol.  in  3  pts.  H2O  (Rammelsberg,  Pogg.  52. 
84) ;  less  sol.  in  H2O  than  SrBr2  -=(-6H2O.  (Lo- 
wig.) 

Thallous  bromate,  TlBrO3. 

SI.  sol.  in  hot  H2O;  easily  sol.  in  HNO3+Aq. 
(Oettinger.) 

Easily  sol.  in  H2O  and  dil.  acids.  (Ditte, 
A.  ch.  (6)  21.  145,) 

Terbium  bromate,  Tb(BrO3)3+9H2O. 

Not  deliquescent.  (Potratz,  C.  N.  1905, 
92,  3.) 

Thallous  bromate,  TlBrO3. 

1  1.  H2O  at  39.75°  dissolves  2.216  x  10-2 
g.  mol.  (Noyes  and  Abbott,  Z.  phys.  Ch. 
1895,  16.  130.) 

SI.  sol.  in  H2O.  3.46  x  10-1  gram  are  con- 
tained in  1  liter  of  sat.  solution  at  20°.  (Bott- 
ger, Z.  phys.  Ch.  1903,  46.  603.) 

Thallic  bromate,  Tl(BrO3)3+3H2O. 

Very  hydroscopic.  Easily  decomp.  by  H20. 
(Gewecke,  Z.  anorg.  1912,  75.  275.) 

Thulium  bromate,  Tm2(BrO3)6  +  18H2O. 

Pptd.  from  sat.  aqueous  solution  by  95% 
alcohol. 

NH4OH  is  the  best  precipitant.  (James, 
J.  Am.  Chem.  Soc.  1911,  33.  1342.) 

Tin  (stannous)  bromate  (?). 

Insol.  in  H2O;  sol.  in  HCl+Aq. 
Uranyl  bromate,  4UO3,  3Br2O6+16H2O. 

Sol.  in  H20.    (Rammelsberg.) 
Yttrium  bromate,  Y(BrO3)3+9H2O. 

More  easily  sol.  in  H2O  than  Y(IO3)3.  SI. 
sol.  in  alcohol.  Insol.  in  ether.  (Cleve.) 

Mpt.  74°.  168  pts.  are  sol.  in  100  pts.  H2O 
at  25°. 

SI.  sol.  in  alcohol.  (James,  J.  Am.  Chem. 
Soc.  1909,  31.  916.) 

Zinc  bromate,  Zn(BrO3)2+6H2O. 

Sol.  in  1  pt.  cold  H2O.  (Rammelsberg, 
Pogg.  52.  90.) 

Zinc  bromate  ammonia,  Zn(BrO3)2,  2NH3  + 
3H2O. 

Decomp.  by  H2O  and  alcohol.  Sol.  in 
NH4OH+Aq.  (Rammelsberg,  Pogg.  52.  90.) 

Zn(Br03)2,  4NH3.  Ppt.  (Ephraim,  B. 
1915,48.51.) 

Perbromic  acid. 
See  Perbromic  acid. 


BROMINE 


119 


Bromides. 

Most  bromides  are  sol.  in  H2O,  many  in 
alcohol,  and  some  in  ether. 

AgBr  and  Hg2Br2  are  insol.  in  H2O  or  acids; 
PbBr2  and  TIBr  are  si.  sol.  therein.  Cu2Br2 
is  insol.  in  H2O,  sol.  in  acids. 

See  under  each  element. 

Bromine,  Br2. 

1  pt.  Br  dissolves  at  15°  in  33  pts.  H2O. 
(Lowig,  Pogg.  14.  485.) 

1  pt.  Br  dissolves  at  15°  in  31  pts.  H2O. 
(Dancer,  Chem.  Soc.  15.  477.) 

Solubility  of  Br  in. 100  pts.  H2O  at  t°. 


t° 

Pts.  Br. 

t° 

Pts.  Br 

t° 

Pts.  Br 

5 
10 

3,600 
3.327 

15 
20 

3.226 
i3.208 

25 
30 

3.167 
3.126 

(Dancer,  /.  c.) 

A  sat.  aqueous  solution  of  Br  contains 
4.05%  Br  at  0°;  3.80%  Br  at  3°;  3.33%Br  at 
10°.  (Roozeboom,  R.  t.  c.  3.  29,  59,  73,  84.) 

1 1.  H2O  dissolves  34  g.  Br  at  25°.  (Jakow- 
kin,  Z.  phys.  Ch.  1896,  20.  25.) 

1  pt.  is  sol.  in  30  pts.  H2O.  (Dietze,  Chem. 
Soc.  1899,  76  (2)  150.) 

100  pts.  H2O  dissolve  at: 

0°  10.34°  19.96°  30.17°  40.03C 
4.167  3.740  3.578  3.437  3.446 
pts.  bromine. 

Liquid  bromine  as  such  is  insol.  in  H20; 
only  the  vapor  dissolves.  (Winkler,  Ch.  Z. 
1899,  23.  688.) 

1 1.  H2O  dissolves  33.95  g.  Br2  at  25°.  (Mc- 
Lauchlan,  Z.  phys.  Ch.  1903,  44.  617.) 

Solubility  of  bromine  vapor  in  H2O  at  tc. 


Solubility  of  bromine  vapor. 
(Mean  of  many  determinations) 

Temp. 

Pressure 

Absorption  coefficient 

0.0 
9.94° 
20.46 
30.38 
40.31 
50.25 
60.04 
69.98 
80.22 

56-13mm. 
80-16 
138-9 
179-12 
229-26 
274-53 
314-46 
154-54 
396-74 

60.53 
35.22 
20.87 
13.65 
9.22 
6.50 
4.84 
3.82 
2.94 

Solubility  of  liquid  bromine. 
(The  mean  of  many  determinations) 

Temp. 

o.° 

10.34° 

19.96° 

30.17° 

40.03° 

49.85° 

Pts.  H2O 
that       , 
dissolve  ' 
1  pt.  Br2 

J4.0 

26.74 

27.94 

29.10 

29.02 

28.38 

Much  less  Br2  is  sol.  in  ice  colid  H2O  in  the 
presence  of  bromine  hydrate. 

Solubility  in  presence  of  bromine  hydrate. 
(The  mean  of  many  determinations) 


49.85° 
3.522 

Temp. 

0°. 

5.12° 

Pts.  H2O  that  dissolve 
1  pt.  Br2 

42.39 

26.26 

(Winkler,  Ch.  Z.  1899,  23.  688-689.) 

Solubility  of  Br2  in  H2O  at  25°  =0.21  mols.- 
in  1  1.  (Bray,  J.  Am.  Chem.  Soc.  1910,  32. 
398.) 

Sp.   gr.   of  Br2+Aq   containing  pts.   Br  in 
10CK)  pts.  solution. 


flS.  BT. 

op.  gr. 

JT  tS.    JDI  . 

Op.    £1. 

t° 

a 

t 

a 

10  72 

1.00901 

18.74-19.06 

1.01491 

0 

60.5 

42 

8.6 

10.68 

1.00931 

19.52-20.09 

1.01585 

2 

54.1 

44 

7.9 

12.05 

1.00995 

20.89-21.55 

1.01807 

4 

,       48.3 

46 

7.4 

12.21 

1.01223 

31.02-31.69 

1.02367 

Q 

43  3 

48 

6.9 

8 

38^9 

50 

6^5 

(Slessor,  N.  Edin.  Phil.  J.  7.  287.) 

10 
12 
14 

35.1 
31.5 

28.4 

52 
54 
56 

6.1 

5.8 
5.4 

Sp.  gr.  of  Br2+Aq  at  32.5°. 
%  Br2  by  weight              Sp.  gr. 

16 

25.7 

58 

5.1 

0.7214 

0.999814 

18 

23.4 

60 

4.9 

1.1172 

1.002520 

20 

21.3 

62 

4.6 

1.6448 

1.006100* 

22 

19.4 

64 

4.4 

1.9956 

1.008870- 

24 

17.7 

66 

4.2 

2.5960 

1.013200 

26 

16.3 

68 

4.0 

(Joseph,  Chem.  Soe.  1915,  107.  3  J 

28 
30 
32 
34 
36 
38 

Af\ 

15.0 
13.8 
12.7 
11.7 
10,9 
10.1 

94 

70 

72 
74 
76 
78 
80 

3.8 
3.6 
3.4 
3.3 
3.1 
3.0 

Sol.  in  cone.  HC1,  HBr,  cone,  solutions  of 
bromides,  and  in  liquid  SO2.     (Sestini,  Zeit. 
Chem.  1868.  718.) 
Much  more  sol.  in  HCl+Aq  than  in  H2O. 
100  com.  HCl+Aq  of  1.153  sp.  gr.  dissolve 
36.4  g.  Br  at  12°. 

40 

.4 

More 

sol.  in  SrCl2,  and  BaCl2+Aq  than  im 

(Winkler,  Ch.  Z-  1899,  23.  688.) 

H2O.    (Berthelot,  C.'  R.  100.  761.) 

120 


BROMINE 


Bromine  is  not  more  sol.  in  KBr-f-Aq  than 
in  H2O  (?).    (Balard.) 
KBr+Aq  containing  1  pt.  KBr  to  6  pts. 
H2O  takes  up  as  much  Br  as  it  already  con- 
tains; when  this  solution  is  heated  the  dis- 
solved Br  is  separated.    1  pt.  KBr+1  pt.  H2O 
takes  up  twice  as  much  Br  as  it  already  con- 
tains, much  heat  being  evolved.    This  solu- 
tion loses  Br  on  exposure  to  the  air  or  when 
heated.    (Lowig.) 

Solubility  of  Br2  in  KBr+Aq. 

Solubility  in  1  liter  Na2SO4+Aq  at  25°. 

NasSO*  +Aq 

g.  Bromine 

1-N 

Vi-N 

Vc-N 
Vs-N 
Vie-N 

25.07 
29.20 
31.33 
32.94 
33.26 

(Jakowkin,  I.  c.) 
Solubility  in  1  liter  NaNO3+Aq  at  25  =\ 

g.  Mols. 
KBr  per  1. 

g.  at.  Br  dissolved 
per  1  at  18.5° 

g.  at.  Br  dissolved 
per  1.  at  26.5°. 

0.00 
0.01 

0.02 
0.03 
0.04 
0.05 
0.06 
0.07 
0.08 
0.09 
0.1 
0.2 
0.3 
0.4 
0.5 
0.6 
0.7 
0.8 
0.9 

0.4448 
0.4634 
0.4823 
0.5049 
0.5243 
0.5431 
0.5668 
0  5895 
0.6059 
0.6301 
0.6533 
0.8718 
1.0549 
1.3124 
1.5436 
1.7712 
2.0006 
2.2354 
2.4851 

0.4282 

0.4490 
0.4671 
0.4925 
0.5101 
0.5301 
0.5530 
0.5636 
0.5920 
0.5981 
0.6488 
0.8591 
1.0787 
1.2704 
1.4731 
1.6717 
1.9197 
2.1C29 
2.3349 

NaNOa+Aq 

g.  Bromine 

1-N 

'A-N 
V4-N 
Vs-N 
Vie-N 

28.80 
31.35 
32.62 
33.33 
33.74 

(Jakowkin,  I.  c.) 
Solubility  in  salts  +Aq  at  25°. 

Salt+Aq. 

g.  Br2  sol.  in  1  liter 

V2-N.Na2SO4 
»/r-N.K«80« 
V2-N.(NH4)2S04 
N.NaNO, 
N.KNO3 
N.NH4NO3 
N.NaCl 
N  KC1 
N.NBUC1 

23.90 
24.80 
77  7 
28  00 
28.95 
55.15 
55.90 
57.40 
82.2 

The  above  figures  indicate  that  below  a 
•concentration  of  0.1  g.  mol.  KBr  per  1.  just 
enough  Br  is  dissolved  to  form  KBr3,  while 
above  that  concentration  somewhat  larger 
amounts  of  Br  are  dissolved,  which  is  greater 
at  the  lower  temp. 
(Worley,  Chem.  Soc.  1905,  87.  1109.) 

(McLauchlan,  Z.  phys.  Ch.  1903,  44.  617.) 

Solubility  in  HgBr2+Aq  at  25°. 
10  prm.  of  t,hf>  solution  nont.ain:  — 

Solubility  of  Br2  in  NaBr+Aq  at  25°. 


g.  NaBr  per  1. 

g.-atoms  Bra  per  1. 

Sp.  gr. 

92.6 

2.479 

1.213 

160.5 

4.345 

1.372 

205.8 

6.195 

1.515 

255.8 

8.575 

1.678 

319.7 

13.65 

1.997 

359.0 

16.04 

2.137 

19.23 

2.327 

408.3 

20.85 

2.420 

(Bell,  J.  Am.  Chem.  Soc.  1912,  34.  14.) 

Solubility  in  salts -j-Aq. 
Solubility  in  1  liter  K2SO4+Aq  at  25°. 


K2SO4+Aq 

g.  Bromine 

1-N 

Vr-N 

V4-N 
Vs-N 
V:e-N 

25.14 
29.44 
31.46 
32.70 
33.10 

(Jakowkin,  Z.  phys.  Ch.  1896,  20,  26.) 


Millimols.  Br2  Millimols.  Hg 

2.125  0. 

2.204  0.0560       , 

2.216  0.0793 

2.226  0.1284 

2.231  0.2120 
(Herz  and  Paul,  Z.  anorg.  1914,  85.  215.) 

1  1.  N.NH4C2H3O2+Aq  dissolves  340.5  g. 
Br2  at  25°.  (McLauchlan,  Z.  phys.  Ch.  1903, 
44.  617.) 

Miscible  in  all  proportions  with  liquid  NO2. 
(Frankland,  Chem.  Soc.  1901,  79.  1361.) 

More  sol.  in  alcohol  than  in  H2O;  miscible 
with  ether,  CS2,  CHC13.  (Sestini,  Zeit.  Chem. 
1868.  718.) 

Somewhat  soluble  in  glycerine.  -  (Pelouze.) 
Sol.  in  benzene  (Mansfield) ;  insol.  in  benzene 
(Moride,  A.  ch.  (3)  39.  452).  Sol.  in  warm 
chloral,  bromal,  and  iodal.  (Lowig,  Pogg.  14. 
485.)  Sol.  in  SC12  (Solly),  and  SBr2.  Sol.  in 
cone.  HC2H3O2+Aq.  (Balard.)  Sol.  in 
aqueous  solution  of  potassium,  sodium,  or  cal- 
cium acetates.  (Cahours.) 


BROMINE 


121 


Solubility  in  CS2. 

100  g.  of  the  sat.  solution  contain  at: 
—95°  —110.5°  —116° 

45.4  39.0  36. 9  g.  Br2. 

(Arctowski,  Z.  anorg.  1896,  11.  274.) 

Cryst.  from  CS2  at  — 90°  in  fine  needles. 
(Arctowski,  Z.  anorg.  1895,  10.  25.) 

Sp.  gr.  of  Br2+CCl4  at  32.5°. 

%  Br2  by  weight  Sp.  gr. 

1 . 5449  1 . 58014 

1 . 6454  1 . 58060 

1 . 7990  1 . 58168 

2 . 6676  1 . 58812 

3 . 5833  1 . 59526 
(Joseph,  Chem.  Soc.  1915,  107.  3.) 

Sp.  gr.  of  Br  2+ nitrobenzene  at  32.5°. 

%  Br2  by  weight  Sp.  gr. 

1.5643  1.20225 

3.2323  1.21449 

4.6462  1.22518 

6 . 1826  1 . 23603 

(Joseph,  Chem.  Soc.  1915,  107.  3.) 

Very  sol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1369.) 

Sol  in  acetone.  (Eidmann,  C.  C.  1899, 
II,  1014;  Naumann,  B.  1904,  37.  4328.) 

Partition  of  Br2  between  water  and  other 

solvents. 
W  =  millimols   Bromine   in    10   ccm.    of   the 

aqueous  layer. 
G=millimols    Bromine    in    10   ccm.    of   the 


A 

C 

N=C/A 

7.545 

691.9 

91.71 

4.109 

338.6 

82.41 

2.660 

217.4 

81.72 

2.544 

207.7 

81.66 

1.740 

140.38 

80.67 

1.2878 

103.7 

80.51 

0.8073 

64.44 

79.83 

0.5046 

39.64 

78.38 

Partition  of  Br2,  etc. — Continued 


Other  solvent 


CS2 


7.750 
10.600 
14.696 
17.999 
26.345 
40.625 
57.038 


1015 
1387 
1910 
2352 
3467 
5194 
7160 


G/w 


76.35 
76.44 
76.98 
76.54 
75.99 
78.21 
79.66 


(Herz,  Z.  Elektrochem,  1910,  16.  871.) 

Partition  coefficient  for  bromine  between  CS2 

and  H2O  at  25°C. 

A  =  concentration  of  the  water  layer. 
C  =  concentration  of  the  CS2  layer. 


Partition    coefficient    for    bromine    between 

CHBr3  and  H2O  at  25°C. 
A  =  concentration  of  the  water  layer. 
C  =  concentration  of  the  CHBr3  layer. 


other  layer. 

A 

C 

N=C/A 

Other  solvent 

G 

w 

G/W 

5.424 
3.838 
2.368 
1.348 
0.766 
0.366 

373.6 
264.7 
161.5 
90.17 
50.49 
23.62 

68.88 
68.80 
68.19 
66.90 
65.84 
64.85 

CC14 

1.949 
7.008 
12.171 
39.880 
54.574 

0.0853 
0.3085 
0.5300 
1.3132 
1.5560 

22.73 
22.71 
23.13 
30.32 
35.01 

Partition  coefficient  for  bromine  between  CC14 
and  H2O  at  25°C. 
A  =  concentration  of  the  water  layer. 
C  =  concentration  of  the  CC14  layer. 

75%  by  vol.  CC14 
+25%  by  vol.  CS2 

3.567 
7.304 
10.833 
13.922 
17.230 
25.637 
40.625 
54.035 

0.0985 
0.1910 
0.2£00 
0.3720 
0.4580 
0.6580 
0.9940 
1.2080 

37.06 
38.15 
37.36 
37.42 
37.62 
38.96 
40.88 
44.73 

A 

C 

N  -C/A 

14.42 
10.80 
7.901 
7.163 
6.803 
5.651 
3.216 
2.054 
1.266 
0.7711 
0.5761 
0.4476 
0.3803 
0.2478 

545.2 
372.2 
252.8 
225.8 
218.5 
172.6 
94.84 
58.36 
35.92 
21.53 
15.72 
12  09 
10.27 
6.691 

37.82 
34.44 
32.01 
31.52 
32.12 
30.54 
29.48 
28.41 
28.37 
27.92 
27.26 
27.02 
27.00 
27.00 

50%  by  vol.  CC14  + 
50%  by  vol.  CS2 

3.592 
6.820 
10.148 
13.866 
16.616 
42.975 
55.965 

0.0784 
0.1487 
0.2206 
0.3065 
0.3688 
0.8086 
0.9960 

45.82 
46.85 
46.01 
45.24 
45.05 
53.15 
56.19 

65.05 
64.82 
65.65 
65.26 
65.17 

25%  by  vol.  CC14 
+75%  by  vol.  CS2 

5.753 
10.902 
26.724 
41.314 
55.526 

0.0884 
0.1682 
0.4970 
0.6331 
0.8520 

(Jakowkin,  Z.  phys.  Ch.  1895,  18.  588;) 

122 


BROMINE  CHLORIDE 


Partition    of    bromine    between    CC14    and 

salts +Aq. 

A  =  concentration  of  Br  in  H2O  layer. 
C  =  concentration  of  Br  in  CC14  layer. 

Partition  of  Br2  between  CC14  and  NaNO3 
Aq  at  25°. 


NaNO3+Aq 

A 

C 

1-N 

V2-N 
Vr-N. 
Vs-N 
Vir-N 

7.905 
8.763 
9.033 
9.200 
9.399 

316.7 
319.5 
315.7 
316.7 
319.3 

(Jakowkin,  Z.  phys.  Ch.  1896,  20,  25.) 

Partition  of  Br2  between  CC14  and  K2SO4  + 
Aq  at  25°. 

K2S04+Aq 

A 

c 

1-N 

V*-N 
Vr-N 

Vs-N 
Vie-N 

5.982 
6.843 
7  354 
7.585 
7.498 

255.4 
253.4 
252.8 
250.3 
242.3 

(Jakowkin,  /.  c.) 

Partition  of  Br2  between  CC14  and  Na2SO4  + 
Aq  at  25°. 

Na2SO4  +Aq 

A 

C 

1-N 

V2-N 
1/4-N 
Vs-N 
Vie-N 

5.934 
6.838 
7.402 
7.609 
7.713 

254.6 
253.4 
254.4 

252.8 
251.2 

(Jakowkin,  I.  c.) 

Crystallizes  at  4°  with  10H2O. 
Bromine  chloride,  BrCl. 

Sol.  in  H2O,  CS2,  ether,  etc. 
Bromine  fluoride,  BrF3. 

Fumes  in  the  air.  Decomp.  by  H2O.  (Le- 
beau,  C.  R.  1905,  141.  1019.) 

Bromine  oxides. 

No  oxides  of  bromine  are  known  in  the  free 
state.  See  hypobromous,  bromic,  and  per- 
bromic  acids. 

Bromiridic  acid. 

Ammonium  bromiridate,  (NH4)2IrBr6. 

Less  sol.  in  cold  H2O  than  the  K  salt. 
(Birnbaum,  Zeit.  Chem.  1865.  22.) 

Very  sol.  in  cold  H2O.  (Gutbier,  B.  1909, 
42.  3910.) 

Caesium  bromiridate,  Cs2IrBr6. 

Sol.  in  H2O.  (Gutbier,  B.  1909,  42.  3911.) 
Potassium  bromiridate,  K2IrBr6. 

Moderately  sol.  in  cold,  more  easily  in  hot 
H2O. 


Insol.  in  alcohol  or  ether. 
Sol.  in  cold  H2O  and  in  HBr+Aq.     (Gut- 
bier, B.  1909,  42.  3910.) 

Rubidium  bromiridate,  Rb2IrBr6. 

Very  sol.   in   cold  H2O.     Sol.  in  hot  dil. 
HBr+Aq.     (Gutbier,  B.  1909,  42.  3911.) 

Sodium  bromiridate.  :  ,; "') 

Deliquescent.    Easily  sol.  in  H20,  alcohol, 
or  ether. 

Bromiridous  acid,  H6Ir2Bri2-f6H2O. 

Easily  sol.  in  H2O,  alcohol,  or  ether.    (Birr- 
baum,  1864.) 

Ammonium  bromiridite,  (NH4)6Ir2Bri2+H2O. 
Difficultly* sol.  in  H2O.    (Birnbaum.) 

Potassium  bromiridite,  K6Ir2Bri2+6H2O. 
Efflorescent.    Sol.  in  H20. 

Silver  bromiridite,  Ag6Ir2Bri2. 
Ppt.    Insol.  in  H2O  or  acids. 

Sodium  bromiridite,  Na6Ir2Bri2+24H2O. 
Efflorescent.    Very  sol.  in  H2O. 

Bromocarbonatoplatmdiamine     carbon- 
ate, ^3[Pt(N2H6)2]2(C03)2+4H20. 
Ppt, 

Bromocarbonatoplatincfo'amine    carbonate 
bromoplatinefo'amine  nitrate, 

B°3[Pt(N2H6)2]2(CC3)2,   2Br2Pt(N2H6)2 
(NO,),. 

BromocWoroplatincfo'amine  chloride, 

g[  Pt(N2H6)2Cl2. 
Very  si.  sol.  in  H2O.    (Cleve.) 

-  chlorobromide,  Q  PtN2H6Br(?)' 
Very  si.  sol.  in  H2O. 
Bromochlororoplatinic  acid. 

Potassium  bromochloroplatinate,  K2PtCl5Br 

(Pitkin,  J.  Am.  Chem.  Soc.  2.  408.) 

Mixture.  (Herty,  J.  Am.  Chem.  Soc.  1896, 
18.  130.) 

K2PtCl4Br2.  SI.  sol.  in  cold  H20;  much 
more  sol.  in  hot  H2O.  (Pitkin.) 

Mixture.    (Herty.) 

K2PtCl3Br3.    As  above. 

K2PtCl2Br4.  (Pigeon,  A.  ch.  1894,  (7)  2. 
488.) 

K2PtClBr5.    (Pitkin.) 

Bromochromic  acid. 

Potassium  bromochromate,  KCrO3Br2  = 

CrO2(Br)OK. 
Decomp.  by  H2O.     (Heintze,  J.  pr.  (2)  4. 


BROMONITRATOPLATINAMINE  NITRATE 


123 


Dibromochromium  chloride, 

[Cr(H2O)4Br2]Cl+2H2O. 
Ppt.    Nearly  insol.  in  fuming  HC1.    (Bjer- 
rum,  B.  1907,  40.  2918.) 

Bromohydroxyloplatincfo'amine   bromide, 


Very  si.  sol.  in  H2O.    (Cleve.) 

--  chloride,  ^  Pt(N2H6Cl)2. 
Sol.  inH2O    (Cleve.) 

-  nitrate,  ^  Pt(N2H6NO3)2. 

Very  si.  sol.  in  cold,  moderately  sol.  in  hot 
H2O.  (Cleve.) 

Bromohydroxyloplatinwonoc&amine 
nitrate,  0>t<«>>+H2O. 
Easily  sol.  in  H2O.    (Cleve.) 
Bromomercurosulphurous  acid. 

Ammonium  bromomercurosulphite, 

NH4SO3HgBr. 
Sol.  in  H2O.    (Earth,  Z.  phys.  Ch.  9.  215.) 

Potassium  bromomercurosulphite, 
KSO3HgBr. 

As  above.    (B.) 

Bromomolybdenum  bromide, 

Br4Mo3Br2  =  molybdenum  efabromide, 
MoBr2. 
Insol.  in  H2O  or  acids,  or  even  in  boiling 

aqua  regia.    Easily  sol.  in  dilute,  decomp.  by 

cone,  alkalies  +Aq.     (Blomstrand,  J.  pr.  82. 

436.) 

Bromomolybdenum    chloride,    Br4Mo3Cl2-|- 

3H2O. 
Insol.  in  acids.    (Blomstrand.) 

Bromomolybdenum  chromate,  Br4Mo3CrO4  + 

2H2O. 

Insol.  in  dil.  acids.  Sol.  in  hot  cone.  HC1 
+Aq.  Insol.  in  alkali  chromates+Aq.  (At- 
terberg.) 

Bromomolybdenum   fluoride,   Br4Mo3F2  + 

3H2O. 
Insol.  in  H2O.    (Atterberg.) 

Bromomolybdenum  hydroxide,  Br4Mo3(OH)2. 

Completely  sol.  in  alkalies  if  not  heated  over 
90°.  (Atterberg.) 

-f  2H2O. 

+8H2O. 

Bromomolybdenum  iodide  hydroxide, 
2Br4Mo3I2,  Br4Mo3(OH)2+8H2O. 

Precipitate.    (Blomstrand,  J.  pr.  77.  92.) 
Bromomolybdenum  molybdate,  Br4Mo3MoO 

Precipitate.    (Atterberg.) 


Bromomolybdenum  phosphate, 

Br4Mo3H4(PO4)2. 
Precipitate.    Insol.  in  H2O.    (Atterberg.) 

Bromomolybdenum    sulphate,   Br4Mo3SO4  + 

3H2O. 

Precipitate.      SI.    sol.    in    boiling    H2SO4. 
(Atterberg.) 

ZH'bromomolybdous  acid,  MoOBr2(OH)  -f 


Sol.  in  H2O.     Very  hydroscopic.  '  (Wein- 
land, Z.  anorg.  1905,  44.  86.) 

!Teirabromomolybdous  acid,  MoBr4(OH)  + 

2H2O. 

Sol.   in  H2O.     Hydroscopic.      (Weinland, 
I.e.) 

D?'ammonium  pewtobromomolybdite, 

MoBr6O(NH4)2. 

Hydroscopic.     Sol.   in  H2O.      (Weinland, 
I.e.) 

Dicsesium  pe«/abromomolybdite, 

MoBr6OCs2. 

Hydroscopic.     Sol.   in  H2O.      (Weinland, 
I.e.) 

Calcium  ^e/rabromomolybdite,   (MoBr4O)2Ca 

+7H2O. 
Hydroscopic.    Sol.  in  H2O.    (Weinland,  I.  c. 


te^rabromomolybdite, 
MoBr4(OLi)+4H2O. 

Hydroscopic.     Sol.   in  H2O.      (Weinland, 
I.e.) 

Magnesium  pewtobromomolybdite, 

MoBr5(OMg)+7H2O. 
Hydroscopic.     Sol.  in  H2O.      (Weinland, 

I.e.) 

M  o  wopotassium  t  efrabromomolybdite, 

MoBr4(OK)+2H2O. 

Hydroscopic.     Sol.  in  H2O.      (Weinland, 
I.e.) 

Dipotassium    pewtobromomolybdite, 

MoBr6OK2. 

Hydroscopic.     Sol.   in  H2O.      (Weinland, 
I.e.) 

Dirubidium  pe«fabromomolybdite, 

MoBr6ORb2. 

Hydroscopic.     Sol.   in  H2O4      (Weinland, 
I.e.) 

Bromonitratoplatindi'amine  nitrate, 

Br  p,N2H6N03. 
NOg    l  N2H6NO3. 
Decomp.  by  H2O.    (Cleve.) 

-  sulphate,  jj£3  Pt(N2H6)2S04+H26. 
SI.  sol.  in  H2O.  ' 


124 


BROMONITRITOPLATINAM1NE  NITRITE 


Bromonitritoplatinsermdi'amine  nitrite, 

NO2Br2Pt(NH3)2NO*, 
SI.  sol.  in  H2O.    (Blomstrand.) 

Bromonitrous  acid. 

Platinum  silver  bromonitrite,  PtAg2Br2(NO2)4. 
Ppt.    (Miolati,  Gazz.  ch.  it.  1900,  30.  588.) 

Bromopalladic  acid. 

Ammonium  bromopalladate,  (NH4)2PdBr6. 

Difficultly  sol.  in  cold  H2O.  Decomp.  by 
hot  H2O  and  by  hot  cone.  H2SO4.  (Gutbier, 
B.  1905,  38.  1907.) 

Caesium  bromopalladate,  Cs2PdBr6. 

Difficultly  sol.  in  cold  H2O.  Decomp.  by 
hot  H2O  or  by  hot  cone.  H2SO4.  (Gutbier, 
I.e.] 

Potassium  bromopalladate,  K2PdBr6. 

Difficultly  sol.  in  cold  H2O.  Decomp.  by 
hot  H2O  or  by  hot  cone.  H2SO4.  (Gutbier, 

I.e.) 

Rubidium  bromopalladate,  Rb2PdBr6. 

Insol.  in  cold  H2O.  Decomp.  by  hot  H20 
or  by  hot  cone.  H2SO4.  (Gutbier,  I.  c.) 

Bromopalladious  acid. 

Ammonium  bromopalladite,  (NH4)2PdBr4. 

Very  stable.  Sol.  in  H2O.  (Smith,  Z. 
anorg.  1894,6.381.) 

Very  sol.  in  cold  H2O. 

Can  be  cryst.  from  a  very  small  amount  of 
hot  H2O.  (Gutbier,  B.  1905,  38.  2387.) 

Barium  bromopalladite. 

Not  deliquescent.  Sol.  in  H2O.  (v.  Bons- 
dorff.) 

Caesium  bromopalladite,  Cs2PdBr4. 

Very  sol.  in  H2O.     (Gutbier,  B.  1905,  38. 

2388.) 

Manganese  bromopalladite,  MnPdBr4. 
Sol.  in  H2O  and  alcohol,    (v.  Bonsdorff.) 
+7H2O.     Very  sol.  in  H2O.     (Smith,  Z. 

anorg.  1894,  6.  382.) 

Potassium  bromopalladite,  K2PdBr4. 

Easily*  sol.  in  H20.  (Joannis,  C.  R.  95. 
295.) 

Very  stable.  Sol.  in  H2O.  (Smith,  Z. 
anorg.  1894,  6.  381.) 

+2H2O.    Unstable  in  the  air.    (Smith,  I.  c.) 

Rubidium  bromopalladite,  Rb2PdBr4. 

Can  be  cryst.  from  a  very  small  amount  of 
hot  H2O.  (Gutbier,  B.  1905,  38.  2388.) 

Sodium  bromopalladite,  Na2PdBr4+4^H2O. 
Very  deliquescent.    Sol,  in  H2O.     (Smith, 
I.e.) 


Strontium  bromopalladite,  SrPdBr4+6H2O. 

Stable  in  the  air.  Very  sol.  in  H2O.  (Smith, 
I.  c.) 

Zinc  bromopalladite. 

Sol.  in  H2O.    (v.  Bonsdorff.) 

Bromophosphatoplatmcfa'amme  phos- 
phate, BrPt(N2H6)2+2H2O. 
\  / 
P04 
SI.  sol.  in  H2O.    (Cleve.) 

Bromopho  sphoric  acid. 

Thorium  bromophosphate,  ThBr4, 

3(3ThO2,  2P2O5). 

Insol.  in  most  acids  and  in  fused  alkali 
carbonates.  Decomp.  by  long  boiling  with 
cone.  H2SO4.  (Colani,  C.  R.  1909,  149.  208.) 

Bromoplatinamine  bromide, 
Br2Pt(NH3Br)2. 

SI.  sol.  in  H2G.  (Cleve,  Sv.  V.  A.  H.  10,  9. 
31.) 

-  nitrite,  Br2Pt(NH3NO2)2. 
Very  si.  sol.  in  H2O.    (Cleve.) 

Bromoplatincfo'amine  bromide, 

Br2Pt(N2H6)2Br2. 
Only  si.  sol.  in  hot  H2O.    (Here.) 

-  chloride,  Br2Pt(N2H6)2Cl2. 
Very  si.  sol.  in  H2O.    (Cleve.) 

-  dichromate,  Br2Pt(N2H6)2Cr2O;. 
SI.  sol.  in  H2O. 

--  nitrate,  Br2Pt(N2H6NO3)2. 

SI.  sol.  in  cold,  rather  easily  sol.  in  hot  H2O. 
(Cleve.) 

--  phosphate,    Br2Pt[N2H6PO2(OH)2]2  + 
2H2O. 

Rather  easily  sol.  in  hot  H2O.    (Cleve.) 

--  sulphate,  Br2Pt(N2H6)2S04. 
Very  si.  sol.  in  H2O. 

Bromoplatinraonocfa'amine  nitrate, 

Rr  Pf  (NH3)2NO3 
BraPt  NH3N03 
.  Easily  sol.  in  H2O. 


--  sulphate,  Br2Pt         .i  SO4+H2O. 
Moderately  sol.  in  H20.     (Cleve.) 

Bromoplatinsemicfa'amine  bromide. 

Br3Pt(NH3)2Br. 
SI.  sol.  in  cold  H2O.    (Cleve.) 

Bromodi'platincfo'amine  anhydronitrate, 


Sol.  in  HNO3+Aq. 


BROMOPURPUREOCHROMIUM  CHLORIDE 


125 


Bromocfa'platincfo'amine  chloride, 

Br2Pt2(N2H€)4Cl4. 
Ppt.    (Cleve.) 

—  nitrate,  Br2Pt2(N2H6)4(NO3)4+2H2O. 
Moderately  sol.  in  hot  H2O. 

-  sulphate,  Br2Pt2(N2H6)4(SO4)2+2H2O. 
"Ppt.    (Cleve.) 

Bromoplatinic  acid,  H2PtBr6+9H2O. 

Very  deliquescent,  and  sol.  in  H2O,  alcohol, 
ether,  chloroform,  or  acetic  acid.  (Topsoe, 
J.  B.  1868.  273.) 

Ammonium  brcmoplatinate,  (NH4)2PtBrG. 
Sol.  in  200  pts.  H2O  at  15°.    (Topsoe.) 
100  pts.  (NH4)2PtBr6+Aq  sat.  at  20°  con- 
tain 0.59  pt.  dry  salt.     (Halberstadt,  B.  17. 

2965.) 

Barium  bromoplatinate,  BaPtBr6  +  10H2O. 
SI.  deliquescent.    Very  sol.  in  H2O. 

Caesium  bromoplatinate,  Cs2PtBr6. 

SI.  sol.  in  dil.  HBr+Aq.  (Obermaier, 
Dissert.) 

Calcium  bromoplatinate,  CaPtBr6  +  12H2O. 
SI.  deliquescent.    Very  sol.  in  H2O. 

Cobalt  bromoplatinate,  CoPtBr6  +  12H2O. 
Deliquescent. 

Copper  bromoplatinate,  CuPtBr6+8H2O. 
Very  deliquescent;  sol.  in  H20. 

Lead  bromoplatinate,  PbPtBr6. 

Easily  sol.  in  H2O,  but  decomp.  by  large 
amount. 

Lead    te/rabromoplatinate,     [PtBr4(OH)2]Pb, 

PbOH. 
Insol.  in  H2O.     (Miolati,  C.  C.  1900,  II. 

810.) 

Magnesium  bromoplatinate,  MgPtBr6  + 

12H20. 
Not  deliquescent. 

Manganese  bromoplatinate,  MnPtBr6  + 

6H2O.  [<rrti  f 

Sol.  in  H2O. 
+  12H2O.    Sol.  in  H2O. 

Mercuric  te/rabromoplatinate, 

[PtBr4(OH)2]Hg 
Insol.  in  H2O.     (Miolati,  C.  C.  1900,  II. 

810.) 

Nickel  bromoplatinate,  NiPtBr6  +  12H2O. 
Deliquescent. 

Potassium  bromoplatinate,  K2PtBr6. 

SI.  sol.  in  H2O.  Insol.  in  alcohol,  (v. 
Bonsdorff,  Pogg.  19.  344.) 


Sol.  in  10  pts.  boiling  H2O.  (Pitkin,  C.  N. 
41.  218.) 

100  pts.  K2PtBr6-f  Aq  sat.  at  20°  contain 
2.02  pts.  dry  salt.  ' (Halberstadt,  B.  17.  2962.) 

Praseodymium  bromoplatinate,  PrBrs,PtBrs 

+  10H2O. 

Deliquescent;  very  sol.  in  H2O;  sol.  in  HBr. 
(Von  Schule,  Z.  anorg.  1898,  18.  353.) 

Rubidium  bromoplatinate,  Rb2PtBr6. 

SI.  sol.  in  dil.  HBr+Aq.  (Obermaier. 
Dissert.) 

Silver  bromoplatinate,  Ag2PtBre. 

Insol.  in  H2O.     (Miolati,  C.  C.  1900,  II. 

810.) 

Silver  tefmbromoplatinate,  [PtBr4(OH)2]Ag2. 
Ppt.;  insol.  in  H2O.    (Miolati,  /.  c.) 

Sodium  bromoplatinate,  Na2PtBr6+6H2O. 
Easily  sol.  in  H2O  and  alcohol. 

Strontium  bromoplatinate,  SrPtBr6  +  10H2O. 
SI.  deliquescent.    Very  sol.  in  H2O. 

Thallium  tefrabromoplatinate, 

[PtBr6(OH)2]Tl2. 

Insol.  in  H2O.  (Miolati,  C.  C.  1900,  II. 
810.) 

Ytterbium   bromoplatinate,  YbBr3,3H2PtBr6 

+30H2O. 
Ppt.    (Cleve,  Z.  anorg.  1902,  32.  138.) 

Zinc  bromoplatinate,  ZnPtBr6+12H2O. 
Sol.  in  H2O. 

Bromoplatinocyanhydiic  acid, 
H2Pt(CN)4Br2. 
See  Perbromoplatinocyanhydric  acid. 

Potassium  bromoplatinocyanide,  5K2Pt(CN)4, 
K2Pt(CN)4Br2  +  18H20. 

Sol.  in  H2O. 
Bromoplatinous  acid. 
Potassium  bromoplatinite,  K2PtBr4+2H2O. 

Extremely  sol.  in  H2O.  (Billmann  and  An- 
dersen, B.  1903,  36.  1566.) 

Bromopurpureo chromium  bromide, 
BrCr(NH3)6Br2. 


Less  sol.  in  H2O  than  chloropurpureo- 
chromium  chloride.  (Jorgensen,  J.  pr.  (2) 
26.  83.) 

bromoplatinate,  BrCr(NH3)5PtBrfi. 

(Jorgensen,  I.  c.) 

chloride,  BrCr(NH3)5Cl2. 

More  sol.  in  H2O  than  the  bromide. 
(Jorgensen,  I.  c.) 


126 


BROMOPURPUREOCHROMIUM  CHROMATE 


Bromcpurpureochromium  chromate, 
BrCr(NH3)5CrO4. 

Precipitate.    (Jorgensen,,  I.  c.) 

-  nitrate,'  BrCr(NH3)5(NO3)2. 

More  sol.  than  bromide  and  less  than 
chloride.  (Jorgensen,  I.  c.) 

Bromopurpureocobaltic  bromide, 

CoBr(NH3)5Br2. 

Sol.  in  530  pts.  H2O  at  16°.  Insol.  in 
alcohol,  NH4Br,  KBr,  or  HBr+Aq.  More 
sol.  in  hot  H2O  containing  a  little  HBr.  (Jor- 
gensen, J.  pr.  (2)  19.  49.) 

Bromopurpureocobaltic    mercuric    bromide, 

CoBr(NH3)5Br2,  3HgBr2. 
More  sol.  in  H2O  than  the  corresponding 
HgCl2salt.    (J.) 

bromoplatinate.      . '  i .  M 

Very  si.  sol.  in  cold  H2O.    (J.) 

-  chloride,  CoBr(NH3)5Cl2. 
Difficultly  sol.  in  cold  H2O,  but  much  more 

easily  than  the  bromide.    Insol.  in  dil.  HC1  + 
Aq,  and  in  alcohol. 

—  mercuric  chloride,  CoBr(NH3)5Cl2, 
3HgCl2. 

SI.  sol.  in  H2O. 
chloroplatinate. 

Nearly  or  quite  insol.  in  H2O.    (J.) 

-  chromate,  CoBr(NH3)6Cr04. 
Nearly  insol.  in  H2O. 

-  dithionate,  CoBr(NH3)5S2O6. 
Nearly  insol.  in  H2O. 

-  fluosilicate,  CoBr(NH3)6SiF6. 

Very  si.  sol.  in  cold  H2O;  insol.  in  alcohol. 

-  nitrate,  CoBr(NH3)5(NO3)2. 

More  sol.  in  H2O  than  the  bromide,  but 
less  than  the  chloride.  Wholly  insol.  in  dil. 
HNO3+Aq  or  alcohol. 

-  oxalate,  CoBr(NH3)5C2O4. 
Nearly  insol.  in  H2O. 

-  sulphate,  CoBr(NH3)5SO4. 

Can  be  crystallized  from  very  dil.  H2SO4  + 
Aq.    Insol.  in  alcohol. 
+6H2O.    Efflorescent. 

Bromopurpureorhodium  bromide, 

BrRh(NH3)5Br2. 

Much  less  easily  sol.  in  H2O  than  the  chloro- 
chloride.  Insol.  in  dil.  HBr+Aq  and  alcohol. 
(Jorgensen,  J.  pr.  (2)  27.  433.) 

-  bromoplatinate,  BrRh(NH3)5PtBr6. 
Almost  insol.  in  H2O. 

-  fluosilicate,  BrRh(NH3)5SiF6. 

SI.  sol.  in  H2O.  Sol.  in  boiling  NaOH+Aq 
as  roseo  salt. 


Bromopurpureorhodium  nitrate, 

BrRh(NH3)5(NO3)2. 

SI.  sol.  in  H2O,  but  much  more  sol.  than  the 
bromide. 

Bromorhodous  acid. 

Ammonium  bromorhodite,  (NH4)2RhBr5. 

Sol.  in  H2O.      (Goloubkine,    Chem.    Soc. 
1911,  100  (2)  45.) 

Sol.  in  H2O.    (Gutbier,  B.  1908,  41.  215.) 

Barium  bromorhodite,  BaRhBr5. 

Sol.  in  H2O.    (Goloubkine,  /.  c.) 
Caesium  bromorhodite,  Cs2RhBr5. 

Difficultly  sol.  in  H2O.    (Gutbier,  I.  c.) 

Potassium  bromorhodite,  K2RhBr5. 
Very  sol.  in  H2O.    (Goloubkine,  I.  c.) 
Sol.  in  H2O.    (Gutbier,  I.  c.) 

Rubidium  bromorhodite,  Rb2RhBrs. 
Sol.  in  H20.    (Goloubkine,  I  c.) 
Difficultly  sol.  in  H2O.     (Gutbier,  I.  c.) 

Sodium  bromorhodite,  Na2RhBr5. 

Very  sol.  in  H2O.    (Goloubkine,  I.  c.) 
Bromoruthenic  acid. 
Potassium  bromoruthenate,  K2RuBr6. 

Very  sol.  in  H2O.     (Howe,  J.  Am.  Chem. 
Soc.  1904,  26.  946.) 

Potassium  agwobromoruthenate, 
K2Ru(H2O)Br5. 

Ppt.    (Howe,  I.  c.) 
Rubidium  bromoruthenate,  Rb2RuBr6. 

Sol.  in  H2O.    (Howe,  /.  c.) 

Rubidium  a^wobromoruthenate, 

Rb2Ru(H2O)Br5. 
Ppt.    (Howe,  /.  c.) 

Bromoruthenious  acid. 

Caesium  bromoruthenite,  CsRuBr5+H2O. 

Ppt.    (Howe,  J.  Am.  Chem.  Soc.  1904,  26. 
945.) 

Potassium  bromoruthenite,  K2RuBrs. 

Very  sol.  in  H2O  with  decomp.    Very  sol. 
in  dil.  HBr.    (Howe,  I.  c.) 

Rubidium  bromoruthenite,  Rb2RuBr5+H2O. 

Sol.  in  dil.  HBr.    (Howe,  /.  c.) 
Bromoselenic  acid. 

Ammonium  bromoselenate,  (NH4)2SeBr6. 

Sol.  in  H2O  with  decomp.    (Muthmann  and 
Schafer,  B.  26.  1008.) 

Caesium  bromoselenate,  Cs2SeBr6. 

SI.  sol.  in  H2O.     (Lenher,  J.  Am.  Chem. 
Soc.  1898,  20.  571.) 

Potassium  bromoselenate,  K2SeBr6. 

As  NH4  salt.    (M.  and  S.) 


BROMOTELLURATE,  AMMONIUM 


127 


Rubidium  bromoselenate,  Rb2SeBr6. 

Less  sol.  in  H2O  than  K  salt.    (Lenher,  I.  c.) 

Bromopj/?*0selenious  acid. 

Ammonium  bromop^/oselenite,  NH4Br,  2SeO2 

+2H20. 

More  easily  sol.  in  H2O  than  corresponding 
Cl  compound.  (Muthmann  and  Schafer,  B. 
1893,  26.  1014.) 

Potassium  bromop?/roselenite,  KBr,  2SeO2  + 

2H2O. 

Sol.  in  H2O.  (Muthmann  and  Schafer,  B. 
26.  1008.) 

Bromosmic  acid. 

Ammonium  bromosmate,  (NH4)2OsBr6. 

Only  si.  sol.  in  H2O.  (Rosenheim,  Z.  anorg. 
1899,  21.  135.) 

Caesium  bromosmate,  Cs2OsBr6. 

Nearly  insol.  in  H2O  and  dil.  HBr.  (Gut- 
bier,  B/1913,  46.  2103.) 

Potassium  bromosmate,  K2OsBr6. 

Only  si.  sol.  in  H2O.    (Rosenheim,  I.  c.) 

Rubidium  bromosmate,  Rb2OsBr6. 

Difficultly  sol.  in  H2O  and  in  dil.  HBr. 
(Gutbier,  /.  c.) 

Silver  bromosmate,  Ag2OsBr6. 

Ppt.;  insol.  in  H2O.    (Rosenheim,  I.  c.) 

Sodium  bromosmate,  Na2OsBr6+4H2O. 
Sol.  in  H2O.    (Rosenheim,  I.  c.) 

Bromostannic  acid,  H2SnBr6 +8H2O. 

Very  deliquescent.  Sol.  in  H2O.  (Seubert, 
B.  20.  794.) 

Ammonium  bromostannate,  (NH4)2SnBr6. 

Very  deliquescent,  and  sol.  in  H2O.  (Ray- 
mann  and  Preis,  A.  223.  323.) 

Caesium  bromostannate. 

Sol.  in  H2O.    (Raymann  and  Preis.) 

Calcium  bromostannate,  CaSnBr6+6H2O. 

Very  deliquescent.  Sol.  in  H2O.  (Ray- 
mann and  Preis.) 

Cobalt  bromostannate,  CoSnBr6  +  10H2O. 

Deliquescent.     (Raymann  and  Preis.) 

Ferrous  bromostannate,  FeSnBre+6H2O. 
Deliquescent.    (Raymann  and  Preis.) 

Lithium  bromostannate,  Li2SnBr6+6H2O. 

Extremely  deliquescent.  (Leteur,  C.  R. 
113.  541.) 

Magnesium  bromostannate,  MgSnBre  + 

10H2O. 
Deliquescent.    (Raymann  and  Preis.) 


Manganous  bromostannate,  MnSnBr6  + 

6H2O. 
Deliquescent.    (Raymann  and  Preis.) 

Nickel  bromostannate,  NiSnBr6+8H2O. 
Deliquescent.     (Raymann  and  Preis.) 

Potassium  bromostannate,  K2SnBr6. 

Sol.  in  H2O.    (Topsoe.) 
Rubidium  bromostannate. 

Sol.  in  H2O.    (Raymann  and  Preis.) 

Sodium  bromostannate,  Na2SnBr6+6H2O. 

Not   deliquescent,    but   extremely   sol.    in 
H2O.    (Seubert,  B.  20.  796.) 

Strontium  bromostannate,  SrSnBr6+6H2O. 

Very  hydroscopic,  and  sol.  in  H2O.    (Ray- 
mann and  Preis.) 

Bromosulphatoplatindi'amine  sulphate, 
rH6)2S04  , 


Rather  easily  sol.  in  hot  H2O. 
Bromosulphobismuthous  acid. 

Cuprous  bromosulphobismuthite,  2Cu2S, 

Bi2S3,  2BiSBr. 

Stable  in  the  air  and  insol.  in  H2O  at  ord. 
temp.  Partially  decomp.  by  boiling  H2O. 
Decomp.  by  mineral  acids  with  the  evolution 
of  H2S.  (Ducatte,  C.  R.  1902,  134.  1212.) 

Lead     bromosulphobismuthite,      PbS,Bi2S3' 

2BiSBr. 

Insol.  in  H2O.  Decomp.  by  boiling  H2O. 
Decomp.  by  dil.  mineral  acids  with  evolution 
of  H2S.  (Ducatte,  I.  c.) 

Bromotantalum  bromide,   (Ta6Bri2)Br2  + 

7H2O. 

Stable  in  the  air  when  in  the  solid  state. 
Sol.  in  H2O  without  decomp.  Sol.  in  propyl 
alcohol.  (Chapin,  J.  Am.  Chem.  Soc.  1910, 
32.  328.) 

Bromotantalum  chloride,  (Ta6Bri2)Cl2  + 
7H2O. 

(Chapin,  I.  c.) 

Bromotantalum  hydroxide,  (Ta6Bri2)(OH)2-f- 
10H2O. 

SI.  sol.  in  HC1.  Stable  in  the  air  below 
100°. 

Sol.  in  alcohol.    Insol.  in  ether.     (Chapin, 
I.e.) 
Bromotantalum  iodide,  (Ta6Br12)I2+7H2O. 

(Chapin,  I.  c.) 
Bromotelluric  acid. 
Ammonium  bromotellurate,  (NH4)2TeBr6. 

Less  sol.  in  H2O  than  K  salt.  (Muthmann 
and  Schmidt,  B.  1893,  26.  1011.) 


128 


BUOMOTELLURATE,  OESIUM 


Caesium  bromotellurate,  Cs2TeBr6. 

Decomp.  by  H2O. 

100  pts.  HBr+Aq  (sp.  gr.  1.49)  dissolve 
0.02  pt.  at  22°. 

100  pts.  HBr+Aq  (sp.  gr.  1.08)  dissolve 
0.13  pt.  at  22°. 

Insol.  in  alcohol.  (Wheeler,  Sill.  Am.  J. 
145.  267.) 

Potassium  bromotellurate,  K2TeBr6+3H2O. 

Sol.  in  little,  decomp.  by  much  H2O.  (v. 
Hauer.) 

Contains  2H2O.  (Wheeler,  Sill.  Am.  J. 
145.  267.) 

Efflorescent. 

100  pts.  HBr+Aq  (sp.  gr.  1.49)  dissolve 
6.57  pts.  at  22°. 

100  pts.  HBr+Aq  (sp.  gr.  1.08)  dissolve 
62. 90  pts.  at  22°. 

Anhydrous.    Stable  on  air.    (Wheeler.) 

Rubidium  bromotellurate,  Rb2TeBre. 

Sol.  in  a  little  hot  H2O,  but  H2TeO3  sep- 
arates on  cooling. 

100  pts.  HBr+Aq  (sp.  gr.  1.49)  dissolve 
0.25  pt.  at  22°. 

100  pts.  HBr+Aq  (sp.  gr.  1.08)  dissolve 
3.88  pts.  at  22°.  (Wheeler.) 

Bromotetramine  chromium  bromide, 

CrBr(NH3)4Br2+H2O. 
Easily  sol.  in  H20.    (Cleve.) 

-  chloride,  CrBr(NH3)4Cl2+H2O. 
Sol.  in  H2O.    (Cleve.) 

-  sulphate,  CrBr(NH3)4SO4+H2O. 
Easily  sol.  in  H20.    (Cleve.) 

Bromotetramine  cobaltic  sulphate, 

BrCo(NH3)4SO4,  or  Br2Co2(NH3)8(SO4)2. 
Sol.  in  H2O.    (Vortmann  and  Blasberg,  B. 
22.  2652.) 

Cadmium,  Cd. 

Not  attacked  by  H2O.  Sol.  in  HC1,  or  dil. 
H2SO4+Aq,  but  more  easily  in  HNO3+Aq. 
Sol.  in  HC2H3O2+Aq. 

Chemically  pure  Cd  like  Zn  is  almost  insol. 
in  dil.  acids,  with  the  exception  of  HNO3 
(Weeren,  B.  1891,  24.  1798.) 

Sol.  in  HClOg+Aq  without  evolution  of  H. 
(Hendrixson,  J.  Am.  Chem.  Soc.  1904  26. 
756.) 

Cadmium  is  sol.  in  molten  CdCl2  and  can 
be  recryst.  therefrom.  (Auerbach.  Z  anorg 
1901,  28.  42.) 

From  4  g.  Cd  in  32  g.  molten  CdCl2  at  650°, 
2.197  g.  were  dissolved  in  */£  hr.  (Helf en- 
stein,  Z.  anorg.  1900,  23.  295.) 

Moderately  quickly  sol.  in  K2S2O8+Aq. 
More  slowly  sol.  in  (NH4)2S2O8+Aq,  (Levi 
Gazz.  ch.  it.  1908,  38  (1)  583.) 

Sol.  in  (NH3)2SiO8+Aq  without  evolution 
of  gas.  (Turrentine,  J.  phys.  Chem.  1907.  11. 
627.) 


Sol.  in  sulphostannates+Aq.  (Storch.  B. 
1883,  16.  2015.) 

%  ccm.  oleic  acid  dissolves  0.0293  g.  Cd  in 
6  days.  (Gates,  J.  phys.  Chem.  1911, 15.  143.) 

Not  attacked  by  sugar  solution.  (Klein 
and  Berg,  C.  R.  102.  1170.) 

Cadmium  amalgam,  Cd2Hg7. 

Stable  from  0°-44°.  Can  be  cryst.  from 
Hg  without  decomp.  if  temp,  does  not  exceed 
44°.  (Kerp.  Z.  anorg.  1900,  25.  68.) 

Cadmium  amide,  Cd(NH2)2. 

Decomp.  by  H2O.  (Bohart,  J.  phys.  Chem. 
1915,  19.  543.) 

Cadmium  arsenide,  Cd3As. 

(Descamps,  C.  R.  86.  1022.) 

Cd3As2.  Sol.  in  dil.  cold  HNO3.  Attacked 
by  aqua  regia.  (Granger,  C.  R.  1904,  138. 

575.) 

Cadmium  azoimide,  Cd(N3)2. 

Ppt.    (Curtius,  J.  pr.  1898,  (2)  68.  294.) 

Cadmium  sw&bromide,  Cd4Br7. 

Decomp.  by  H2O.  (Morse  and  Jones,  Am. 
Ch.  J.  1890,  12.  490.) 

Cadmium  bromide,  CdBr2. 

Deliquescent.    Very  sol.  in  H2O. 

Solubility  in  H2O  at  t° 


t° 

%  CdBr2 

t° 

%  CdBr2 

—4 

32.0 

48 

60.0 

—1 

34.7 

71 

61.2 

+  1 

36.3 

104 

61.8 

2 

36.0 

155 

63.7 

9 

41.9 

170 

65.2 

14 

46.0 

215 

69.9 

25 

52.6 

232 

70.1 

35 

59.6 

245 

71.5 

Solid  phase  above  100°  is  CdBr2-.  _, . 
(Etard,  A.  ch.  1894,  (7)  2.  541.) 
See  also  under  CdBr2+H2O  and  CdBr2  + 
4H2O. 

Sp.  gr.  of  CdBr2+Aq  at  19.5°  containing: 
5  10          15          20  25  %  CdBr2, 

1.043     1.090     1.141     1.199     1.260 
30         35          40         45  50  %  CdBr2. 

1.326     1.400     1.481     1.5*78     1.680 
(Kremers,  calculated  by  Gerlach,  Z.  anal.  8. 
280.) 

CdBr2+Aq  containing  18.06%  CdBr2  has 
sp.  gr.  20°/20°  =  1.1378. 

CdBr2+Aq  containing  21.39%  CdBr2  has 
sp.  gr.  20°/20°  =  1.1666. 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  282.) 

Sp.  gr.  of  CdBr2+Aq  containing  35.84% 
CdBr2  =  1.4231  at  19.4°/4°.  (Hallwachs,  W. 
Ann.  1899,  68.  27.) 


CADMIUM  RUBIDIUM  BROMIDE 


129 


Sp.  gr.  of  CdBr2+Aq  at  18°/4°. 
%CdBr2        33.289     23.973     20.552     11.983 
Sp.gr.  1.384       1.252       1.209       1.112 

%CdBr2         6.543      3.734       1.927 
Sp.  gr.  1.106       1.030       1.017 

(de  Muynck,  W.  Ann.  1894,  53.  561.) 

Sp.  gr.  of  CdBr2+Aq  at  18°. 
%  CdBr2      1  5  10         15         20 

Sp.  gr.        1.0072  1.0431  1.0907  1.1432  1.1991 

%  CdBr2      25         30         35         40         43 
Sp.  gr.        1.2605  1.3296  1.4052  1.4915  1.5467 
(Grotrian,  W.  Ann.  1883,  18.  193.) 
•  Sp.  gr.  of  CdBr2+Aq. 


%  CdBr2 

t° 

Sp.  gr.  at  t° 

Sp.  gr.  at  18° 

0.0324 

17 

.90 

0.99901 

0.99900 

22 

.75 

0.99702 

0.0748 

17 

.23 

0.99949 

0.99935 

21 

.50 

0.99863 

0.154 

17 

.67 

1.00008 

1.00002 

23 

.10 

0.99896 

0.253 

17 

.23 

1.00119 

0.00100 

22.95 

0.99986 

0.506 

18.07 

0.00308 

1.00310 

22 

.65 

1.00212 

1.013 

18 

.00 

1.00750 

(Wershofen, 

Z.  phys.  Ch.  1890,  6.  493.) 

Sp.  gr. 

of  CdBr2+Aq  at  20°. 

Normality  of 
CciBn  +Aq 

%CdBr2 

Sp.  gr. 

2.774 

46.574 

1.6198 

1.997 

37.53 

1.4469 

0.973 

22.53 

1.2293 

0.5138 

12.46 

1.1211 

(Forchheimer,  Z.  phys.  Ch.  1900,  34.  29.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Sol.  in  AlBr3.  (Isbekow,  Z.  anorg.  1913, 
84,  27.) 

Sol.  in  HCl+Aq,  HC2H3O2,  alcohol,  or 
ether.  (Berthemot,  A.  ch.  44.  387.) 

Sol.  in  0.94  pt.  H2O,  3.4  pts.  abs.  alcohol, 
250  pts.  ether,  and  16  pts.  alcohol-ether  (1:1) 
(Eder,  Dingl.  221.  89.) 

Anhydrous  CdBr2  is  sol.  in  acetone.  (Krug 
and  M'Elroy.) 

1  g.  CdBr2  is  sol.  in  64.5  g.  acetone  at  18°. 
Sp.  gr.  of  sat.  solution  18°/4°  =  0.8073.  (Nau- 
mann, B.  1904,  37.  4337.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014.) 

Insol.  in  mustard  oil.  (Mathews,  J.  phys. 
Chem.  1905,  9,  647.) 

Difficultly  sol.  in  methyl  acetate.  (Nau- 
mann,  B.  1909,  42,  3790.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

Sol.  in  chinoline.  (Beckmann  an'd  Gabel, 
Z.  anorg.  1906,  51.  236.) 

100  g.  benzonitrile  dissolve  0.857  g.  CdBr2 
at  18°.  (Naumann,  B.  1914,  47.  1370.) 


Mol.    weight    determined    in    piperidine. 
(Ferchland,  Z.  anorg.  1897,  15,  17.) 
+H2O.    Solubility  in  H2O. 
100  g.  of  the  sat.  solution  contain  at: 
35°     40°     45°     60°     80°    100° 
60.29  60.65  60.75  61.10  61.29  61.63  g.  CdBr2. 
(Dietz,  Z.  anorg.  1899,  20.  261.) 

+  1KH2O.    (fitard,  A.  ch.  1894,  (7)  2.  541.) 
+4H2O.       Efflorescent.       (Rammelsberg, 
Pogg.  55.  241.) 
Solubility  in  H2O. 
100  g.  of  the  sat.  solution  contain  at: 

0°        18°        30°        38° 
37.92     48.90     56.90    61.84  g.  CdBr2. 
Sp.  gr.  of  sat.  solution  at  18°  =  1.683. 
(Dietz,  Z.  anorg.  1899,  20.  261.) 

100  g.  sat.  solution  of  CdBr2+4H2O  in 
absolute  alcohol  contain  20.93  g.  CdBr2  at 
15°. 

100  g.  sat.  solution  of  CdBr2+4H20  in 
absolute  ether  contain  0.4  g.  CdBr2  at  15°. 
(Eder,  Dingl.  221.  89.) 

Cadmium  hydrogen  bromide. 

Decomp.  by  H2O.  (Berthelot,  C.  R.  91. 
1024.) 

Cadmium  caesium  bromide,  CdBr2,  CsBr. 

Easily  sol.  in  H2O.  (Wells  and  Walden,  Z. 
anorg.  6.  270.) 

CdBr2,  2CsBr.  Decomp.  by  H2O  into 
above  comp.  (W.  and  W.) 

CdBr2,3CsBr.  Decomp.  by  H2O  into 
CdBr2,  CsBr.  .(W.  and  W.) 

Cadmium  potassium  bromide,  CdBr2,  KBr  + 


Sol.  in  0.79  pt.  H2O  at  15°;  pptd.  by  alcohol 
and  ether.  (Eder,  Dingl.  221.  89.) 

+H2O.  Sol.  in  H2O  without  decomp.  from 
0.4°-112.5°.  (Rimbach,  B.  1905,  38,  1554.) 

100  pts.  of  the  solution  contain  at: 
0.4°     15.8°       50°      112.5° 
53.75     58.68     68.25      78.10  pts.  of  the  salt. 

CdBr2,  4KBr.  Sol.  in  1.40  pts.  H2O  at  15°; 
pptd.  by  alcohol  and  ether.  (Eder,  Dingl. 
221.  89.) 

Cannot  be  prepared  in  a  pure  state  as  it  is 
decomp.  by  H2O  below  160°.     (Rimbach,  B.. 
1905,  38.  1560.) 
Cadmium  rubidium  bromide,  CdBr2,  RbBr.. 

Sol.  in  H2O  without  decomp.  from  0.4°  to 
107.5°. 

100  pts.  of  the  solution  contain  at: 

0.4°     14.5°     49.2°     107.5° 
32.65     41.87     58.54      75.77  pts.  of  the  salt. 
(Rimbach,  B.  1905,  38.  1556.) 

CdBr2,  4RbBr.  Sol.  in  H2O  without 
decomp.  from  0.5°  to  114.5°. 

100  pts.  of  the  solution  contain  at: 
0.5°     13.5°     51.5°     114.5° 
47.95     55.17     68.82       79.04  pts.  of  the  salt.. 
(Rimbach,  B.  1905,  38.  1561.) 


130 


CADMIUM  SODIUM  BROMIDE 


Cadmium  sodium  bromide,  CdBr2,  NaBr  + 


Sol.  at  15°  in  1.04  pts.  H2O,  3.7  pts.  abs. 
alcohol,  and  190  pts.  ether  (sp.  gr.  0.729). 
(Eder,  Dingl.  221.  89.) 

3CdBr2,  2NaBr+6H2O.  Stable  in  cone, 
solutions  and  decomp.  only  by  great  dilution. 
(Jones  and  Knight,  Am.  Ch.  J.  1899,  22.  134.) 

Cadmium  bromide  ammonia,  CdBr2,  2NH3. 

Can  be  crystallized  out  of  warm  NH4OH  + 
Aq.  (Croft,  Phil.  Mag.  21.  356.) 

CdBr2,  3NH3.  (Tassily,  C.  R.  1897,  124. 
1022.) 

CdBr2,  4NH3.    Decomp.  by  H2O.    (Croft.) 

Cadmium  bromide  cupric  oxide,  CdBr2, 
3CuO+3H2O.  (Mailhe,  A.  ch.  1902,  (7) 
27.  383.) 

Cadmium  bromide  hydrazine,  CdBr2,  2N2H4. 
Easily  sol.  in  NH4OH+Aq.    (Franzen,  Z. 
anorg.  1908,  60.  280.) 

Cadmium    bromide    hydroxylamine,    CdBr2, 

2NH2OH. 

Sol.  in  hot  H2O  with  formation  of  a  basic 
salt.  Sol.  in  dil.  acids.  Insol.  in  alcohol  and 
ether.  (Adams,  Am.  Ch.  J.  1902,  28.  218.) 

Cadmium  sw&chloride,  Cd4Cl7. 

Decomp.  by  H2O  and  by  acids.  (Morse 
and  Jones,  Am.  Ch.  J.  1890,  12.  490.) 

Cadmium  chloride,  CdCl2. 

Sol.  at  20°  40°    60°      80°     100° 

in  0.71  0.72  0.72    0.70    0.67  pts.  H2O. 


CdCl2+Aq  containing  8.91%  CdCl2  has 
sp.  gr.  20°/20°  =  1.0715.  (Le  Blanc  and 
Rohland,  Z.  phys.  Ch.  1896,  19.  282.) 

Sp.  gr.  of  CdCl2-|-Aq  at.  room  temp,  con- 
fining: 

^CdClo  11.09       16.30    24.786 

p.  gr.    "  1.1093     1.1813     1.3199 

(Wagner,  W.  Ann.  1883,  18.  266.) 

Sp.  gr.  of  CdCla+Aq  at  18°/4°. 
%CdCl2  57.524    41.547     29.977 

Sp.gr.  1.852       1.515       1.330 

CdCl2  21.431         14.761 

Sp.gr.  1.210  1.142 

(de  Muynck,  W.  Ann.  1894,  53.  561.) 

Sp.  gr.  of  CdCl2+Aq  at  18°. 


%  CdCl2 

1 

5 

•   10 

15 

%CdCt2 

1.0063 
20 

1.0436 
25 

1.0919 
30 

1.1443 
35 

%CdCl2 

1.2007 
40 

1.2620 
45 

1.3305 
50 

1.4075 

Sp.  gr. 

1.4878 

1.5775 

1.6799 

(Grotrian,  W.  Ann.  1883,  18.  193.) 

Sp.  gr.  of  CdCl2+Aq  at  25°. 

Concentration  of  CdCl2+Aq  Sp.  gr. 

1-normal  1.0779 

V2-      "  1.0394 

V4-      "  1.0197 

Vs-      "  1.0098 

(Wagner,  Z.  phys.  Ch.  1890,  5.  36.) 

Sp.  gr.  of  CdCl2+Aq. 


Sat.  CdCl2+Aq  contains  %  CdCl2  at  t°. 

%CdCl2 

t° 

Sp.  gr.  at  t° 

Sp.  gr.  at  18° 

00503 
0.0999 
0.200 
0.399 
0.599 
0.769 
0.997 

17.59 
24.27 
17.70 
22.06 
18.31 
24.00 
16.86 
24.21 
17.49 
25.12 
17.58 
21.76 
17.55 
19.65 

0.99920 
0.99781 
0.99964 
0.99833 
1.00038 
0.99920 
1.00239 
1.00083 
1.00406 
1.00238 
1.00580 
1.00496 
1.00754 
1.00713 

0.99910 
0.99958 
1.00044 
1.0022 
1.0039 
1.0057 
1.0075 

t° 

%CdCl2 

t° 

%CdCl2 

—7 

6 
7 
10 
19 
25 
61 
82 

43.5 
47.6 
49.7 
51.3 
51.6 
52.7 
52.9 
57.9 
58.8 

120 
150 
165 
170 
180 
190 
200 
235 
270 

63.0 
64.8 
68.2 
68.4 
70.1 
71.9 
72.0 
76.0 
77.7 

(fitard,  A.  ch.  1894,  (7)  2.  536.) 

100  mol.  H2O  dissolve  at: 
19.3°     29.7°     40.1°     54.5° 
10.94     12.74     13.15     13.16  mol.  CdCl2. 
(Sudhaus,  Miner.  Jahrb.  Beil.-Bd.  1914,  37. 
19.) 
See    also    under     CdCl2+H2O,     CdCl2  + 
2^H2O,  and  CdCl2+4H20. 

gp.  gr.  of  CdCl2+Aq  containing  pts.  CdCl2 
to  100  pts.  H2O. 
13          26.9         41      pts.  CdCl2, 
1.1068     1.2106     1.3100 
55.8        72.5         114.2  pts.  CdCl2. 
1.4060     1.5060     1.7266 
(Kremers,  Fogg.  103.  57.) 

(Wershofen,  Z.  phys.  Ch.  1890,  5.  4.92.) 
Sp.  gr.  of  CdCl2+Aqatt°. 

t° 

Normality  of 
CdCl2+Aq 

g.  CdChin           Sp.,gr. 
100  g.  of  solution       t°/4° 

20.5 

3.80 
2.61 
1.76 
1.29 
0.93 
0.52 

44.42              1.5645 
34.22              1.3941 
25.90              1.2435 
19.91              1.1977 
14.88              1.1404 
8.84              1.0801 

(Oppenheimer,  Z.  phys.  Ch.  1898,  27.  454.) 

CADMIUM  CHLORIDE 


131 


Sp.  gr.  of  CdCl2+Aqatt°. 

Solubility  in  Na'Cl-j-Aq  at  t°. 

t° 

Concentration  of  CdCh+Aq 

Sp.  gr. 

t 

100  g.  H2O  dissolve 

Solid  phase 

22 

18.7 
17.2 
16 
17 
22 

1  pt.  CdCl2  in  1.3458  pts.  H2O 
1    '                "  2.7005       ' 
1    '               "  53.988       ' 
1    '                "  54.18 
1    '                "  57.479       ' 
1    '                "  77.232      ' 

1.6128 
.2896 
.0155 
.0152 
.0136 
.0076 

g.  CdCh 

g.    NaCl 

19.3 

29.7 

111.30 
116.64 

85.15 
40.01 
5.96 

7.52 

12.19 
25.67 
36.76 

35.84 

CdCh+2HH2O 
CdCh  +2^H2O  +CdCh, 
2NaCl+3H20 
CdCh,  2NaCl+3H20 

CdCh,  2NaCl+3H20  + 
NaCl 
NaCl 

(Hittorf,  Z.  phys.  Ch.  1902,  39.  628.) 
Solubility  in  KCl+Aq  at  t°. 

129.65 
132.67 

123.54 
106.16 
91.10 
43  74 
9.43 

9'.63 

10.10 
12.92 
15.41 
27.46 
37.54 

35.88 

CdCh+2^H2O 
CdCh  +2^H20  +CdCh, 
2NaCl+3H2O 
CdCh,  2NaCl  +3H2O 

CdCh,  2NaCl  +3H2O  + 
NaCl 
NaCl 

t° 

00  g.  H2O  dissolve 

Solid  phase 

g.  CdCh 

g.  KCl 

19.3 

111.30 
59.59 

26.98 
11.61 

1.44 

6.70 

11.09 
30.04 

34.76 
33.94 

CdCU+2J4HiO 

CdCh+2HH20+CdCh, 
KCl+HzO 
CdCh,  KC1+H20 
CdCh,  KCl  +H2O  +CdCl2, 
4KC1 
CdCh,  4KC1+KC1 
KCl 

40.1 

133.85 

137.03 

48.17 
13.31 

15  '.14 

29.50 
38.16 

36.18 

CdCh+H20 
CdCh+H2O+CdCh, 
2NaCl+3H20 
CdCh,  2NaCl+3H2O 
CdCh,  2NaCl+3H2O  + 
NaCl 
NaCl 

29.7 

129.65 

97.62 
68.23 

47.12 
32.67 
24.26 
15.99 
15.47 

2.42 

0.70 
7.08 

9.89 
13.06 
16.10 
25.97 
33.58 

37.66 
37.21 

CdCh+3HH20 
CdCh+2^H20 
CdCh  +2^H20  +CdCl2, 
KC1+H2O 
CdCh,  KCl  +H20 

CdCh,  KCl+HtO+CdCU, 
4KC1 
CdCh,  4KC1  +KC1 
KCl 

54.5 

133.90 
140.42 

52.76 
22.53 

19.10 

32.97 
39.  G7 

36.82 

CdCh+H20 
CdCh  +H2O  +CdCh, 
2NaCl+3H2O 
CdCh,  2NaCl+3H20 
CdCh,  2NaCl+3H2O  + 
NaCl 
NaCl 

At  34.5°,  Cdri2+2KH20-»CdCl2+H20  and 
water. 
(Sudhaus,  Miner.  Jahrb.  Beil.-Bd.  1914,  37. 

28.) 

Insol.   in  SbCl3.      (Klemensiewicz,   C.   A. 
1909,  269.) 
Insol.  in  liquid  NH3.     (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 
Insol.  or  si.  sol.  in  ethyl  alcohol,  furfurol, 
acetophenone,  ethyl  monochloracetate,  ethyl 
cyanacetate,    ethyl    oxalate,    ethyl    nitrate, 
amyl  nitrite,  o-nitrotoluene,  pyndme,  pipen- 
dine,  and  quinoline.     Sol.  in  salicylic  alde- 
hyde.   (Lincoln,  J.  phys.  Chem.  1899,  3.  461.) 
Insol.  in  anhydrous  ether.     (Hampe,  Ch. 
Z.  1887,  II,  847.) 
Readily  sol.  in  alcohol. 
100  pts.  absolute  methyl  alcohol  dissolve 
1.71  pts.  CdCla  at  15.5°. 
100  pts.  absolute  ethyl  alcohol  dissolve  1.52 
pts.  CdCl2  at  15.5°.    (de  Bruyn,  Z.  phys.  Ch. 

100  g.  CdCl2+CH3OH  contain  1.5  g.  CdCl2. 

40.1 

133.85 
92.15 

51.90 
37.91 
24.45 
18.97 
19.92 

2.98 

2.70 

11.50 
15.21 
21.73 
35.51 
37.63 

40.45 
40.36 

CdCh+H2O 
CdCh+H20+CdCh, 
KCl  +H2O 
CdCh,  KC1+H-O 

CdCh,  KCl  +H2O  +CdCh, 
.4KC1 
CdCh,  4KC1  +KC1 
KCl 

54.5 

133.90 
102.15 

44.01 
26.13 

4.20 

2  32 

18.39 

43.78 

45.52 
43.00 

CdCh+H2O 
CdCU+HjO+CdCU, 
KCl  +H2O 
CdCh,  KCl  +H2O 
CdCh,  KCl+HjO+CdClj 
4KC1 
CdCh,  4KC1  +KC1 
KCl 

(Sudhaus,  Miner.  Jahrb.  Beil.-Bd. 
34.) 

1914,  37 

132 


CADMIUM  HYDROGEN  CHLORIDE 


at  the  critical  temp.    (Centnerszwer,  Z.  phys 
Ch.  1910,  72.  437.) 

Somewhat    sol.    in    acetone.      (Krug    and 
M'Elroy.) 

Sol.  in  acetone;  insol.  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II,  1014.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Sol.  in  ethyl  acetate.  (Naumann,  B.  1904, 
37.  3601.) 

Difficultly  sol.  in  ethylacetate.  (Naumann, 
B.  1910,  43.  314.) 

Sol.  in  urethane.  (Castoro,  Z.  anorg.  1899, 
20.  61.) 

At  18°,  100  g.  benzonitrile  dissolve  0.06332 
g.  CdCl2.  (Naumann,  B.  1914,  47,  1370.) 

Insol.  in  toluene.  (Baxter  and  Hines,  Am. 
Ch.  J.  1904,  31.  222.) 

Sol.  in  chinolin.  (Beckmann  and  Gabel, 
Z.  anorg.  1906,  51.  236.) 

+H2O.    Solubility  in  H2O. 

100  g.  of  the  sat.  solution  contain  at: 
10°  20°  40°  60° 

57.47        57.35        57.51         57.77 

80°          100° 
58.41         59.52  g.  CdCl2. 

110°  is  bpt.  of  the  sat.  solution. 

(Dietz,  Z.  anorg.  1899,  20.  257.) 

+2J^H2O.    Solubility  in  H2O. 
100  g.  of  the  sat.  solution  contain  at: 
—10°      0°          18°        30°        36° 
44.35     47.37     52.53     56.27    57.91  g.  CdCl2. 
Sp.  gr.  of  sat.  solution  =  1.741. 
(Dietz,  Z.  anorg.  1899,  20.  257.) 

+4H2O.    Solubility  in  H2O. 

100  g.  of  the  sat.  solution  contain  at: 
—9°        0°        +10°     +15° 
43.58    49.39     55.58    59.12  g.  CdCl2. 
(Dietz,  Z.  anorg.  1899,  20.  257.) 

+5H2O.  (Worobieff,  Z.  anorg.  1898,  18. 
386.) 

Cadmium  hydrogen  chloride,  CdCl2,  2HC1  + 

7H20. 

Decomp.  in  air.  (Berthelot,  C.  R.  91. 
1024.) 

Cadmium  caesium  chloride,  CdCl2,  2CsCl. 

Easily  sol.  in  H2O  and  dil.  HCl+Aq;  insol. 
in  cone.  HCl+Aq.  (Godeffroy,  B.  8.  9.) 

Nearly  insol.  in  CsCl+Aq.  (Wells  and 
Walden,  Z.  anorg.  5.  266.) 

CdCl2,  CsCl.  SI.  sol.  in  H2O;  nearly  insol. 
inCdCl2+Aq.  (Wells  and  Walden.) 

Cadmium  calcium  chloride,  2CdCl2,  CaCl2  + 
7H2O. 

Rather  deliquescent,  and  very  sol.  in  H2O. 
When  ignited  is  only  si.  sol.  in  H2O  with 
evolution  of  heat.  (v.  Hauer,  J.  pr.  63.  432.) 

CdCl2,  2CaCl2  +  12H2O.  Very  deliques- 
cent, (v.  Hauer.) 


Cadmium  cobaltous  chloride,  2CdCl2,  CoCL 
+  12H20. 

Deliquescent.  Sol.  in  H2O.  (v.  Hauer  W 
A.  B.  17.  331.) 

Cadmium   cupric   chloride,   CdCl2,    CuCl2  + 

4H2O. 
Sol.  in  H2O.    (v.  Hauer,  W.  A.  B.  17.  331.) 

Cadmium  hydrazine  chloride,  CdCl2. 
N2H4HC1. 

Unstable  in  the  air  when  moist.  Very  sol. 
in  H2O;  si.  sol.  in  alcohol;  sol.  in  NH3+Aq. 
(Curtius,  J.  pr.  1894,  (2)  50.  334.) 

CdCl2,2N2H4HCl+4H2O.      Very    sol.    in 


H2O;  si.  sol.  in  alcohol.    (Curtius, 
(2)  50.  335.) 


y    so 
J.  pr. 


1894, 


Cadmium   iron    (ferrous)    chloride,   2CdCl2, 

FeCl2+12H2O. 
Sol.  in  H2O.    (v.  Hauer,  W.  A.  B.  17.  331.) 

Cadmium   lithium   chloride,    CdCl2,    LiCl  + 


Very  deliquescent.  Decomp.  by  solution 
in  H2O,  but  not  in  alcohol.  (Chassevant,  A. 
ch.  (6)  30.  39.) 

Cadmium  magnesium  chloride,  2CdCl2, 

MgCl2  +  12H2O. 

Deliquescent  in  moist,  stable  in  dry  air. 
Easily  sol.  in  H2O  with  absorption  of  heat. 
Much  more  sol.  in  hot  than  in  cold  H2O.  (v. 
Hauer.) 

Solubility  in  H2O  at  t°. 


t° 

G.  CdjAlgCh  in 
100  g.  solution 

G.  Cd2MgCl5  in 
100  g.  H2O 

24 

45.61 

83.86 

20.8 

49.69 

98.77 

45.5 

53.51 

115.10 

67.2 

58.14 

138.90 

121.8 

65.48 

189.69 

(Rimbach,  B.  1897,  30.  3084.) 

CdCl2,    2MgCl2  +  12H2O.      Very   deliques- 
cent,   (v.  Hauer.) 

Cadmium  manganese   chloride,   2CdClo, 
MnCl2  +  12H2O. 

Deliquescent  in  moist,  efflorescent  in  dry 
air.    Sol.  in  H2O.    (v.  Hauer.) 

Cadmium  nickel  chloride,  CdCl2,  2NiCl2  + 

12H2O. 

Sol.  in  H2O.    (v.  Hauer,  W.  A.  B.  20.  40.) 
2CdCl2,  NiCl2  +  12H2O.    Sol.  in  H2O.     (v. 

Hauer.) 

Cadmium  potassium  chloride,  CdCl2,  KC1  + 


Sol.  in  H2O  without  decomp.    (v.  Hauer.) 


CADMIUM  CHLORIDE  AMMONIA 


133 


+H2O.    100  mol.  H2O  dissolve  at: 
19.3°  29.7°  40.1°  54.5° 

2.65   3.21   3.72   4.33  mol.  CdCl2,  KCl-fH2O. 
(Sudhaus,  Miner.  Jahrb.  Beil.-Bd.  1914,  37. 

26.) 


Cadmium  rubidium  chloride,  CdCl2,  2RbCl. 

Sol.  in  H2O  and  HCl+Aq.  (Godeffroy,  B. 
8.9.) 

CdCl2,  RbCl.    Solubility  in  H2O  at  t°. 

100  pts.  by  wt.  of  the  solution  contain  pts. 
by  wt.  RbCl,  CdCl2. 


_ 

t° 

Pts.  RbCl,  CdCU 

t° 

G.  CdKCh  in 
100  g.  solution 

G.  CdKCh  in 
100  g.  H20 

1.2 
14.5 
41.4 
57.6 
103.9 

12.97 
16.80 
25.31 
30.83 
46.62 

2.6 
15.9 
41.5 
60.6 
105.1 

21.87 
26.60 
35.66 
40.67 
51.67 

27.99 
36.  4 
55.34 
68.55 
106.91 

CdCl2,  RbCl  is  sol.  in  H2O  without  decomp. 
from  0-104°.    (Rimbach,  B.  1902,  35.  1303.) 

(Rimbach,  B.  1897,  30.  3079.) 

CdCl2,  2KC1.     100  pts.  H2O  at  15.5°  dis- 
solve 33.45  pts.     SI.  sol.  in  alcohol.     (Croft, 
Phil.  Mag.  (3)  21.  356.) 
Solubility  in  salts+Aq  at  16°. 
CdCl2,  2KC1  is  sol.  without  decomp.  in  the 
following  salt  solutions  at  16°. 

vxi^i2,  'in.D^i. 

Solubility  of  CdCl2,  4RbCl  and  CdCl2,  RbCi 
in  H2O  at  t°. 

t° 

In  100  pts.  by  wt.  of 
the  solution 

Composition  of 
the  solid  phase 

Pts.  by 

wt.  Cd 

Pts.  by 
wt.  Cl 

Pts.  by 
wt.  Rb 

Mol.-% 
mono- 
salt 

Mol.-% 
tetra- 
salt 

70 
76 
84 
86 
67 

Salt 

Mols. 
salt  in 
100  mole 
H20 

In  1  litre  of  the  solution 
mole 

Sp.  gr. 
of  the 
solution 

1.1380 
1.2333 
1.214 

CdCh 

KCl 

RCl 

0.7 
8.8 
13.8 
42.4 
59.0 
108.4 

0.65 
1.07 
1.32 
3.21 
4.61 
8.94 

6,52 
7.37 
7.86 
11.35 
13.41 
18.57 

14.73 
16.13 
16.93 
22.45 
25.31 
31.15 

30 
24 
16 
14 
33 

LiCl 

CaCl2 
KC1 

9.3 

3.8 

2.378 

0.166 
0.270 
0.507 

0.663 
1.080 
3.195 

4.483 

1.887 

(Rimbach,  B.  1905,  38.  1568,) 
CdCl2,    4KC1.      More   sol.    in   H2O    than 

(Rimbach,  B.  1902,  35.  1305.) 

CdCl2,  KCl.    (v.  Hauer.) 

100  g.  H2O  dissolve  at: 

19.3°     29.7°     40.1°       54.5° 

41.65     49.05     57.55      69.91  g.  CdCl2,  4KC1. 

(Sudhaus,  Miner.  Jahrb.  Beil.-Bd.  1914,  37. 

24.) 

Solubility  in  H2O  at  t°. 


t° 

100  pts.  solution  contain  pts. 

Cd 

Cl 

K 

4.0 
23.6 
50.2 
108.8 
109.0 

3.64 
5.66 
9.10 
11.97 
11.91 

9.84 
14.02 
18.09 
23.08 
23.15 

8.31 
11.52 
13.60 
17.10 
17.22 

(Rimbach,  B.  1897,  30.  3080.) 

Decomp.  by  H2O. 

Can  be  recryst.  without  decomp.  from  LiCl, 
CaCl2,  or  MgCl2+Aq.  (Rimbach,  B.  1905, 
38.  1565.) 

The  salt  is  sol.  without  decomp.  in  HCl+Aq 
containing  19.8  mole  HC1  per  100  mole  H2O 
at  16C. 

1  1.  of  the  solution  contains  0.033  mole 
CdCl2,  0.132  mole  KCl  and  8.828  mole  HC1; 
sp.  gr.  of  the  solution  =  1.1 403.  (Rimbach, 
B.  1905,  38.  1568.) 


Decomp.   by  H2O   between  0°  and    108°. 
(Rimbach,  B.  1905,  38.  1571.) 

Sol.  in  cone.  HC1  without  decomp.    (Rim 
bach,  B.  1905,  38.  1571.) 

Not  sol.  in  CaCl2+Aq  and  LiCl+Aq  with- 
out decomp.    (Rimbach,  B.  1905,  38.  1571.) 

Cadmium  sodium  chloride,  CdCl2,  2NaCl-f- 

3H2O. 

Sol.  in  1.4  pts.  H2O  at  16°.    (Croft.) 
100  mol.  H2O  dissolve  at: 
193°        29.7°        40.1°        54.5° 
3  93          4.29          4.73          5.18  mol.  CdCl2, 

2NaCl+3H2O. 
Stable  between  19°  and  55°. 
(Sudhaus,  Miner.  Jahrb.  Beil.-Bd.  1914,  37. 

25.) 
SI.  sol.  in  alcohol  or  wood  alcohol.    (Croft.) 

Cadmium  strontium  chloride,  2CdCl2,  SrCl2  + 

7H2O. 
Sol.  in  H2O.    (v.  Hauer.) 

Cadmium  chloride  ammonia,  CdCl2,  2NHa. 

Nearly  insol.  in  H2O.    (v.  Hauer.) 

CdCl2,  3NH3-f-^H2G. 

CdCl2,  4NH3  +  ^H2O. 

CdCl2,  5NH3.    (Andre,  C.  R.  104.  908.) 

CdCl2,  6NH3.    Difficultly  sol.  in  cold  H2O. 
(Schiller,  A.  87.  34.) 


134 


CADMIUM  CHLORIDE  CUPRIC  OXIDE 


Cadmium     chloride     cupric     oxide,     CdCl2, 

3CuO+3H2O. 

Not  decomp.  by  H2O.  (Mailhe,  A.  ch. 
1902,  (7)  27.  378  and  174.) 

Cadmium  chloride  hydrazine,  CdCl2,  2N2H4. 
Insol.  in  H2O. 
Sol.  in  NH4OH+Aq.     (Franzen,  Z.  anorg. 

1908,  60.  279.) 

+H2O.  Insol.  in  H2O;  easily  sol.  in 
NH4OH+Aq.  (Curtius,  J.  pr.  1894,  (2)  60. 
345.) 

Cadmium  chloride  hydroxylamine,  CdCl2, 
2NH2OH. 

SI.  sol.  in  cold,  somewhat  more  in  warm 
H2O.  yery  sol.  in  hydroxylamine -j-Aq.  Very 
si.  sol.  in  alcohol  and  other  organic  solvents. 
(Crismer,  Bull.  Soc.  (3)  3.  116.)  . 

Aq  solution  sat.  at  20°  contains  about  1%. 
(Antonoff,  C.  C.  1905,  II.  810.) 

Cadmium  fluoride,  CdF2. 

Difficultly  sol.  in  H2O.  Easily  sol.  in  HF  + 
Aq.  (Berzelius,  Pogg.  1.  26.) 

Very  sol.  .in  H2O;  insol.  in  95%  alcohol; 
sol.  in  HC1,  H2SO4,  or  HNO3+Aq  with  evolu- 
tion of  HF.  (Poulenc,  C.  R.  116.  582.) 

1  1.  H2O  dissolves  0.289  mol.  CdF2  at  25°, 
or  100  cc.  sat.  aqueous  solution  contains  4.36 
g.  CdF2  at  25°.  (Jaeger,  Z.  anorg.  1901,  27. 
35.) 

1  1.  of  1.08-N  HF  dissolves  0.372  mol. 
CdF2  at  25°.  (Jaeger,  Z.  anorg.  1901,  27.  35.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  827.) 

Cadmium  eerie  fluoride,  CdF2,2CeF4+7H2O. 
Ppt.     Decomp.  by  H2O.     (Rimbach,   A. 

1909,  368.  106.) 

Cadmium  columbium  fluoride. 
See  Fluocolumbate,  cadmium. 

Cadmium  molybdenyl  fluoride. 
See.Fluoxymolybdate,  cadmium. 

Cadmium  silicon  fluoride. 
See  Fluosilicate,  cadmium. 

Cadmium  stannic  fluoride. 
See  Fluostannate,  cadmium. 

Cadmium  titanium  fluoride. 

See  Fluotitanate,  cadmium. 
Cadmium  zirconium  fluoride. 

See  Fluozirconate,  cadmium. 
Cadmous  hydroxide,  CdOH. 

Insol.  in  H2O.  Decomp.  by  acids  into 
cadmic  salt.  (Morse  and  Jones,  Am.  Ch.  J. 
12.  488.) 

Cadmium  hydroxide,  CdO2H2. 
Insol.  in  H2O. 
1 1.  CdO2H2+Aq  contains  0.0026  g.  CdO2H2 


at  25°.  (Bodlander,  Z.  phys.  Ch.  1898,  27. 
66.) 

Solubility  in  H2O  =  2.6  x  10-4.  (Herz,  Z. 
anorg.  1900,  24.  126.) 

Sol.  in  acids;  very  sol.  in  NH4OH+Aq; 
insol.  in  KOH,  NaOH,  Na2CO3,  K2CO3,  and 
(NH4)2CO3+Aq. 

Easily  sol.  in  (NH4)2SO4,  NH4C1,  NH4NO3, 
and  NH4  succinate+Aq.  (Wittstein.) 

Freshly  pptd.  CdO2H2  is  sol.  in  alkali 
haloids +Aq.  (Bersch,  Z.  phys.  Ch.  1891,  8. 
392.) 

Solubility  in  NH4OH+Aq  increases  with 
increase  in  concentration  of  NH4OH.  (Euler, 
B.  1903,  36.  3401.) 

Solubility  in  NH4OH+Aq  at  25°. 


NHs  norm. 

g.  CdO  per  1. 

0  5 

0.24 

1.0 

0.62 

1.8 

1.33 

4.6 

4.92 

(Bonsdorff,  Z.  anorg.  1904,  41.  187.) 

Insol.  in  ethyl,  and  methyl  amine+Aq. 
(Wurtz.) 

Very  si.  sol.  in  HCN  +  Aq  even  when  freshly 
pptd.  (Schiiler,  A.  87.  48.) 

Not  pptd.  in  presence  of  Na  citrate  (Spiller), 
and  many  non-volatile  organic  substances. 
(Rose.) 

Cadmium  iodide,  CdI2. 

Sol.  in  1.13  pts.  H2O  at  15°.  (Eder,  Dingl. 
221.  89.) 

Sol.  at    20°    40°    60°     80°   100° 

in  1.08  1.00  0.93  0.86  0.75  pts.  H2O. 

(Kremers,  Pogg.  103.  57.) 


Sat.  CdI2+Aq  contains  at: 

—4°  +2°  +10°    13°  24° 

42.4  43.7  45.2     44.8  46.5 
54°  64°  76°      94°  95° 

49.5  50.1  52.4     55.1  54.7 
140°  165°  185°    202°  202° 
63.1  68.1  70.7 


32° 

47.4%  CdI2. 

135° 

62.9%  CdI2. 

255° 

Cdlo. 


(fitard,  A.  ch.  1894,  (7)  2.  545.) 

Solubility  in  H2O. 

100  g.  of  the  sat.  solution  contain  at: 

0°         18°         50°         75°       100° 
44.39     46.02     49.35     52.65     56.08  g.  CdI2. 
(Dietz,  Z.  anorg.  1899,  20.  262.) 

Sp.  gr.  of  Cd  I2+Aq  containing  pts.  CdI2  to 
100  pts.  H2O. 

21.4  43.7  88.5  pts.  CdI2. 

1.1681         1.328         1.6139 

(Kremers,  Pogg.  111.  60.) 


CADMIUM  IODIDE 


135 


Sp.  gr.  of  CdI2+Aq  at  19.5°  containing: 
5  10          15          20         25  %CdI2, 

1.044     1.088     1.138     1.194     1.253 


50  %CdI2. 
1.680 


30         35         40         45 
1.319     1.395     1.476     1.575 
(Kremers,   calculated   by   Gerlach,   Z.   anal. 
8.  285.) 

Sp.  gr.  of  CdI2+Aq  at  18°. 
%  CdI2        1  5          10          15         20 

Sp.  gr.     1.0071  1.0425  1.0883  1.1392  1.1943 

%  CdI2      25          30         35          40         45 
Sp.  gr.     1.2550  1.3228  1.4000  1.4816  1.5741 
(Grotrian,  W.  Ann.  1883,  18.  193.) 

Sp..gr.  of  CdI2+Aq. 


g.CdI2per  1. 

Sp.  gr. 

g.CdI2  per  1. 

Sp.gr. 

98.85 

197.7 

1.08 
1.162 

289.5 
400 

1.237 
1.328 

(Barbier  and  Roux,  Bull.  Soc.  1890,  (3)  3. 
425.) 

Sp.  gr.  of  CdI2+Aq. 


0.0429 
0.100 
0.204 
0.399 

0.600 
0.800 

1.00 


17.68 
22.88 
17.55 
22.91 
17.76 
22.79 
17.40 
24.30 
18.00 
17.44 
23.11 
18.00 


Sp.  gr.  at  t°     Sp.  gr.  at  18° 


0.99915 
0.99807 
0.99965 
0.99363 
1.00052 
0.99948 
0.00223 
1.00082 

1.00564 
1.00442 


0.99908 
0.99956 
1.0005 
1.0021 

1.0038 
1.0056 

1.0072 


CdI2+Aq  containing  1  pt.  CdI2  in  2.2691 
pts.  H2O  at  17°  has  sp.  gr.  =  1.3341.  (Hit- 
torf,  Z.  phys.  Ch.  1902,  39.  628.) 

Sol.  in  sat.  HI+Aq. 

Sol.  in  warm  NH4OH+Aq. 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  827.) 

.  SI.  sol.  in  liquid  NH3.    (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Sol.  in  S2C12.  (Walden,  Z.  anorg.  1900,  25. 
217.) 

Difficultly  sol.  in  POC13.  (Walden,  Z. 
anorg.  1900,  25.  212.) 

Nearly  insol.  in  AsBr3.  (Walden,  Z.  anorg. 
1902,  29.  374.) 

Sol.  in  SO2C12.  (Walden,  Z.  anorg.  1900, 
25.  215.) 

Sol.  in  15  pts.  alcohol.  (Vogel,  N.  Rep. 
Pharm.  12.  393.) 

Sol.  in  0.98  pt.  abs.  alcohol.  (Eder,  Dingl. 
221.  89.) 

Sp.  gr.  of  CdI2+ alcohol. 

%CdI2  Sp.  gr.  20°/20° 

0  0.7949 

7.28  0.8470 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  284.) 

Sol.  in  5.2  mols.  methyl,  7  mols.  ethyl,  and 
9.8  mols.  propyl  alcohol  at  20°.  (Timofejew, 
C.  R.  112.  1224.) 

Sol.  in  3.6  pts.  ether.    (Eder,  I.  c.) 

Sol.  in  2.0  pts.  alcohol-ether  (1  :  1).  (Eder, 
I.e.) 

Very  si.  sol.  in  anhydrous  abs.  ether. 
(Hampe,  Ch.  Z.  1887,  11.  847.) 

100  g.  of  sat.  solution  in  abs.  ether  contain 
0.143  g.  CdI2  at  12°.  (Tyrer,  Proc.  Chem. 
Soc.  1911,  27.  142.) 

Solubility  in  ether +Aq  at  12°. 


2° 


(Wershofen,  Z.  phys.  Ch.  1890,  5.  493.) 

Sp.  gr.  CdI2+Aq  at  18°/4°  containing: 
31.123         13.677        9.559  %  CdI2. 

1.338  1.125         1.086 

(de  Muynck,  W.  Ann.  1894,  53.  561.) 

CdI2+Aq  containing  10.97%  CdI2  has  sp. 
gr.  20°/20°  =  1.0982. 

CdI2+Aq  containing  16.53%  CdI2  has  sp. 
gr.  20°/20°  =  1.1562. 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  282.) 

Sp.  gr.  of  CdI2+Aq  at  20°. 


0.0 

0.10 

0.30 


0.143 

0.78 

2.07 


0.50 
0.70 
0.90 


3.36 

4.77 
6.46 


1.00 
1.10 
1.14 


7.30 

8.27 
8.68 


(Tyrer,  Proc.  Chem.  Soc.  27.  142.) 
Solubility  in  benzene       at  16°    =0.01% 
"   35°    =0.02% 

Solubility  in  ethyl  ether  at  0°  =0.03% 
"  15.5°  =  0.04% 
"  20.3°  =0.05% 

(Linebarger,  Am.  J.  Sci.  1895,  (3)  49.  52.) 
Sol.  in  acetone.    (Eidmann,  C.  C.  1899,  II. 
1014.) 

1  g.  CdI2  is  sol.  in  4  g.  acetone  at  18°. 
Sp.  gr.  of  sat.  solution  18°/4°  =  0.994.    (Nau- 


Normality  of 
CdI2+Aq 

%   CdI2 

Sp.  gr. 

mann,  B.  1904,  37.  4338.) 
Sp.  gr.  of  CdI2+acetone. 

1.924 
0.951 

0.447 
0.211 

44.53 
27.07 
14.40 
7.26 

1.5807 
1.2837 
1.1355 
1.0630 

%CdI2 

Sp.  gr.  20°/20°. 

0 
12.02 

0.7998 
0.8929 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  284.) 

(Forchheimer,  Z.  phys.  Ch.  1900,  34.  29.) 

136 


CADMIUM  HYDROGEN  IODIDE 


Sol.  in  chinolin.  (Beckmann  and  Gabel, 
Z.  anorg.  1906,  61.  236.) 

100  g.  benzonitrile  dissolve  1.6295  g.  CdI2 
at  18°.  (Naumann,  B.  1914,  47.  1370.) 

Insol.  in  methylene  iodide.  (Retgers,  Z. 
anorg.  3.  343.) 

SI.  sol.  in  ethylamine.  (Shinn,  J.  phys. 
Chem.  1907,  11.  538.) 

Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1849, 
6.  257.) 

Solubility  in  methyl  acetate  =  0.7-1.5%; 
2.1%  at  bpt.  (Schroder  and  Steiner,  J.  pr. 
1909,  (2)  79.  49.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

1  pt.  is  sol.  in  54.3  pts.  ethyl  acetate  at  18°. 

The  sat.  solution  has  D18°/4°  =  09i45 
(Naumann,  B.  1910,  43.  318.) 

Insol.  in  mustard  oil.  (Mathews,  J.  phys. 
Chem.  1905,  9.  647.) 

Mol.  weight  determined  in  piperidine, 
pyridine,  methyl  and  ethyl  sulphide.  (Wer- 
ner, Z.  anorg.  1897,  15.  17.) 

Cadmium  hydrogen  iodide,  CdI2,  HI+3H2O. 
Decomp.    in   air.      (Dobroserdow,    C.    C. 
1900,  II.  527.) 

Cadmium  caesium  iodide,  CdI2,  CsI+H2O. 

Sol.  in  H2O  without  decomp.  (Wells  and 
Walden,  Z.  anorg.  5.  271.) 

CdI2,  2CsI.    As  above. 

CdI2,  3CsI.  Decomp.  by  H2O  into  the 
above  salt. 

Cadmium  hydrazine  iodide,  CdI2,2N2H4HI. 
Sol.  in  H2O.    (Ferratini,  C.  A.  1912. 1612.) 

Cadmium  mercuric  iodide. 

Very  sol.  in  H2O.  (Berthemot,  J.  Pharm 
14.  613.) 

CdI2,  3HgI2.  Sol.  in  H2O.  Can  be  re- 
crystallized  in  alcohol.  (Clarke  and  Kebler 
Am.  Ch.  J.  6.  235.) 

Cadmium  potassium  iodide,  CdI2,  KI+H2O. 
Sol.  in  0.94  pt.  H2O  at  15°.    (Eder,  Dingl. 

C*dI2,  2KI+2H2O.  Deliquescent.  Ex- 
tremely sol.  in  H2O.  Sol.  at  15°  in  0.73  pt. 
H2O.  SI.  sol.  in  alcohol  and  wood  spirit,  but 
less  than  CdI2.  (Croft.) 

Sol.  at  15°  in  1.4  pts.  absolute  alcohol,  24.5 
pts.  ether  (0.729  sp.  gr.),  and  4.5  pts.  alcohol- 
ether  (1  :  1).  (Eder,  I.  c.) 

Sp.  gr.  of  K2CdI4+Aq  at  18°. 
%K2CdI4       1  5         10         15         20 

Sp.  gr.        1.0065  1.0384  1.0808  1.1269  1.1770 

%K2CdI4     25         30         35         40         45 
Sp.  gr.        1.2313  1.2890  1.3557  1.4282  1.5065 
(Grotrian,  W.  Ann.  1883,  18.  193.) 


Sp.  gr.  of  K2CdI4+Aq. 


%K2Cdl4 

t° 

Sp.  gr.  at  t° 

Sp.  gr.  at  18° 

0.0328 

18 

0.99895 

0.0596 

18 

0.99921 

0.0804 

18 

0.99938 

0.100 

17.12 

0.99962 

0.99945 

21.82 

0.99872 

0.250 

18 

1.0007 

0.500 

18 

1.0027 

1.003 

17.32 

1.0068 

1.0067 

20.63 

1.0061 

(Wershofen,  Z.  phys.  Ch.  1890,  5.  493.) 

Sol.  in  ethyl  acetate.  (Naumann,  B.  1904, 
37.  3601.) 

Cadmium  sodium  iodide,  CdI2,  2NaI+6H2O. 

Deliquescent.    (Croft.) 

Sol.  at  15°  in  0.63  pt.  H2O,  0.86  pt.  abs. 
alcohol,  and  10.1  pts.  ether  (sp.  gr.  0.729). 
(Eder,  Dingl.  221.  89.) 

Cadmium    strontium    iodide,    CdI2,    SrI2-h 
8H2O. 

Deliquesces  in  moist,  effloresces  in  dry  air: 
sol.  in  H2O.  (Croft.) 

Cadmium  iodide  ammonia,  CdI2,  2NH3. 
Decomp.  by  H2O.    (Rammelsberg.) 
CdI2,  4NH3.    (Dawson  and  McCrae,  Chem. 
Soc.  1900,  77.  1246.) 

CdI2,  6NH3.  Decomp:  by  H2O;  sol.  in 
warm,  less  sol.  in  cold  NH4OH+Aq.  (Ram- 
melsberg.) 

Cadmium  iodide  hydrazine,  CdI2,  2N2H4. 

Easily  sol.  in  warm  NH4OH+Aq.  (Fran- 
zen,  Z.  anorg.  1908,  60.  281.) 

Cadmium    iodide    hydroxylamine,    CdI2, 
3NH2OH. 

Sol.  in  H2O  and  alcohol.  Insol.  in  ether. 
(Adams,  Am.  Ch.  J.  1902,  28.  218.) 

Cadmium  iodide  selenide,  CdI2,  3CdSe. 

Easily  decomp.  (Fonzes-Diacon,  C.  R. 
1900,  131.  897.) 

Cadmium  iodosulphide,  Cdl,  2CdS. 
Ppt.    (Naumann,  B.  1904,  37.  4338.) 

Cadmium  sw&oxide,  Cd4O. 

Decomp.  by  H2O,  acids  and  NH4OH-f- 
Aq.  (Tanatar,  Z.  anorg.  1901,  27.  433.) 

Cd2O.  Properties  as  cadmous  hydroxide. 
(Morse  and  Jones.) 

Cadmium  oxide,  CdO. 

Insol.  in  H2O.  Sol.  in  acids.  Sol.  in 
NH4OH+Aq.  Insol.  in  (NH4),CO3-fAq. 
Easily  sol.  in  NH4Cl+Aq,  less  in  NH4NO3-|- 
Aq.  (Brett,  1837.) 


CADMIUM  SULPHIDE 


137 


Insol.  in  KOH,  NaOH,  K2CO3,  and  Na2CO3 
+Aq. 
See  also  Cadmium  hydroxide. 

Solubility  in  (calcium  sucrate+ sugar)  + 
Aq. 

1  1.  solution  containing  418.6  g.  sugar  and 
34.3  g.  CaO  dissolves  0.22  g.  CdO. 

1  1.  solution  containing  174.4  g.  sugar  and 
14.1  g.  CaO  dissolves  0.48  g.  CdO. 

(Bodenbender,  J.  B.  1866.  600.) 

Insol.  in  acetone.    (Naumann,  B.  1904,  37. 

Insol.  in  methyl  acetate.  (Naumann,  B 
1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1904,  37.  3601.) 

Cadmium  peroxide,  Cd5O8  or  Cd3O5(?). 

(Haas.) 

CdO2,  Cd(OH)2.  (Kouriloff,  A.  ch.  (6)  23. 
431.) 

Very  stable  towards  H2O.  Insol.  in  NH4OH 
+Aq.  (Haas,  B.  1884,  17.  2253.) 

4CdO2,  Cd(OH)2.  Ppt.  Insol.  in  NaOH  + 
Aq.  (Eykmann,  C.  C.  1905,  I.  1629.) 

5CdO2,CdO+3H2O.  Ppt.  (Teletow,  C.  A. 
1912,  43.) 

Cadmium  oxybromide,  CdO,  CdBr2+H2O. 

Decomp.  by  H2O.  (Tassily,  C.  R.  1897, 
124.  1023.) 

+2H2O.  Stable  in  dry  air;  insol.  in  H2O. 
(Tassily,  C.  R.  1897,  124.  1022.) 

+3H2O.  Slowly  decomp.  by  H2O.  (Tas- 
sily, C.  R.  1897,  124.  1022.) 

+7H2O.    (Mailhe,  C.  R.  1901,  132.  1561.) 

Cadmium  oxychloride,  CdCl2,  CdO+H2O. 

SI.  sol.  in  hot  H2O.  (Habermann,  M.  Ch. 
5.  432.) 

+7H2O.  (Mailhe,  Bull.  Soc.  1901,  (3)  25. 
791.) 

2CdO,  CdCl2.  Insol.  in  H2O,  but  slowly 
decomp.  thereby.  (Canzoneri,  Gazz.  ch.  it. 
1897,  27.  (2)  486.) 

Cadmium  oxyiodide,  CdO,  CdI2+H2O. 

Decomp.  by  H2O.  (Tassily,  C.  R.  1897, 
124.  1023.) 

+3H2O.  Stable  in  dry  air;  insol.  in  H2O. 
(Tassily,  C.  R.  1897,  124.  1022.) 

Cadmium  phosphide,  Cd3P2. 

Sol.  in  HCl+Aq  with  evolution  of  PH3. 
(Stromeyer.) 

Cd2P."  Sol.  in  cone.  HCl+Aq.  (Emmer- 
ling,  B.  12.  152.) 

Easily  decomp.  by  acids.  (Kulisch,  A.  231. 
327.) 

CdP-.  Decomp.  by  boiling  cone.  HCl+Aq. 
(Renault,  C.  R.  76.  283.) 

Cadmium  selenide,  CdSe. 

Sol.  in  HCl+Aq.    (Uelsmann,  A.  116.  122.) 
Easily  decomp.  by  acids.    (Fonzes-Diacon, 

C.  R.  1900,  131.  897.) 


Cadmium  sulphide,  CdS. 

Insol.  in  H2O. 

Solubility  in  H2O  at  16- 18°  =  6.6  x  10-6 
mols  per  1.  (Biltz,  Z.  phys.  Ch.  1907,  58. 

291.) 

1  1.  H2O  dissolves  9.00  x  10-6  mols.  CdS 
(artificial  greenockite)  at  18°. 

1  1.  H2O  dissolves  8.86  x  10-6  mols.  pptd. 
at  18°.    (Weigel,  Z.  phys.  Ch.  1907,  58. 

Difficultly  sol.  in  hot  dil.  HCl+Aq.  Easily 
sol.  in  cold  cone.  HCl+Aq.  (Stromeyer.) 
Sol.  in  HNO3+Aq  (Meissner),  and  boiling  dil. 
H2S04+Aq  (1:6).  (A.  W.  Hoffmann,  A. 
115.  286.)  Very  si.  sol.  in  NH4OH+Aq. 
(Wackenroder,  Repert.  46.  226.)  Insol  in 
KOH,  or  (NH4)2S+Aq.  Appreciably  sol.  in 
an  acid  solution  of  NH4C1.  (Baxter  and 
Hines,  Z.  anorg.  1905,  44.  160.) 

Much  more  sol.  in  (NH4)2S+Aq  than  us- 
ually supposed.  (Ditte,  C.  R.  86.  402.).  Sol- 
ubility increases  by  warming,  and  at  68°  is 
twice  that  at  ordinary  temperatures.  A  sat. 
solution  of  (NH4)2S  dissolves  about  2  g.  CdS 
to  a  litre.  Alkali  sulphides  dissolve  much 
less.  (Ditte.) 

Fresenius  (Z.  anal.  20.  236)  could  not  con- 
firm the  above.  According  to  Fresenius,  CdS 
is  not  appreciably  sol.  in  (NH4)2S+Aq. 

Insol  in  Na2SO3  or  KCN  +  Aq.    (Fresenius.) 

Insol.  in  NH4C1  or  NH4NO3  +  Aq.    (Brett.) 

Sol.  in  alkali  sulpho-molybdates,  -tung- 
states,  -vanadates,  -arsenates,  -antimonates, 
-stannates+Aq.  (Storch,  B.  16.  2015.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37.' 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

Min.  Greenockite.    Sol.  in  HCl+Aq. 

Colloidal. — Solution  of  4  g.  colloidal  C 
in  a  litre  H2O  remains  transparent  several 
days.  If  it  contains  11  g.  CdS  in  a  litre,  it  is 
completely  coagulated  in  24  hours.  Solutions 
of  salts  of  the  following  concentration  cause 
an  immediate  coagulation  in  an  aqueous  solu- 
tion of  CdS  containing  3.62  g.  in  a  litre. 


KC1 
KBr      . 
KI 
KCN    . 

KC1O3  . 
KNO3  . 

K2S206 

K2SO,  . 

K3Fe(CN)6 

K4Fe(CN)6 

K2CrO4 

K2Cr207 

NaCl    . 

Na2S2O3 

NaHCO3 

Na2CO3 

Na2HP04 


1615 

727 

57 

166 

1666 

1000 

5000 

833 

166 

100 

400 

3571 

2666 

98 

333 

166 

202 


138 


CADMIUM  SULPHIDE 


NaC2H302     .         .     1 

2451 

Caesium  ammonia,  Cs,NH3. 

Na  benzoate          .     1 

10,000 

Sol.  in  liquid  NH3.    (Moissan,  C.  R.  1903, 

(NH4)2C204.        .     1 

588 

136.  1177.) 

BaCl2   ...     1 

11,764 

Ba(NO3)2      .         .     1 

8032 

Caesium  azoimide,  CsN3. 

BaS2O6          .         .     1 
MgSO4          .         .     1 
MnSO4          .         .     1 

5617 
41,666 
22,222 

Deliquescent.    Stable  in  aq.  solution. 
224.2  pts.  sol.  in  100  pts.        H2O        at    0° 
307.4     "     "      ..  100    "          H2O         "  16° 

CdSO4  ...     1 

250,000 

1.0366     "     "      "  100    "    abs.  alcohol  "  16° 

Cd(N03)2     .        .     1 
Pb(C103)2     .        .     1 

285,714 
209 

Insol.  in  pure  ether.     (Curtius,  J.  pr.  1898, 
(2)  58.  283.) 

Pb(C2H3O2)2         .     1 

147,058 

Hg(CN)2       .         .<! 

20 

Caesium  bromide,  CsBr. 

A12(SO4)3      .        .     1 
Alum    .       ,  .         .1 
Chrome  alum        .     1 
HC1      ...     1 

232,558 
192,377 
42,555 
4807 

Ppt.    (Chabrie,  C.  R.  1901,  132.  679.) 
Sat.    CsBr+Aq   at   25°    contains   55.23% 
CsBr.    (Foote,  Am.  Ch.  J.  1907,  37.  125.) 

H2SO4  ...     1 
HC2H3Oo      .         .     1 

8000 
15 

Caesium  fnbromide,  CsBr3. 

H2C2O4  "      .         .1 

23,255 

Sol  in  H2O;  decomp.  by  alcohols.    (Wells, 

Succinic  acid         .  <  1 

100 

Sill.  Am.  J.  143.  17.) 

Tartaric  acid         .     1 

333 

(Prost,  Belg.  Acad.  Bull.  (3) 
1887.  537.) 

14.  312;  J.  B. 

Caesium  pe«Zabromide,  CsBr5. 
Very  unstable.     (Wells  and  Wheeler,  Sill. 

Am.  J.  144.  42.) 

Cadmium  pentasulphide,  CdS8. 
Insol.  in  H2O.    (Schiff,  A.  116.  74.) 
Mixture  of  CdS  and  S.    (Follenius,  Z.  anal. 

13.  412.) 

Cadmium  potassium  sulphide,  K2Cd3S4. 
(Milbauer,  Z.  anorg.  1904,  42.  439.) 

Cadmium  sodium  sulphide,  3CdS,  Na2S. 

Decomp.  by  H2O.  (Schneider,  J.  pr.  (2) 
0.  29.) 

Cadmium  sulphoiodide. 
See  Cadmium  iodosulphide. 

Cadmium  telluride,  CdTe. 

Not  attacked  by  dil.  acids.  Attacked  in 
the  cold  only  by  HNO3.  (Tibbals,  J.  Am. 
Chem.  Soc.  1909,  31.  908.) 

Cadmic  acid. 

Potassium  cadmate. 

Insol.  in  H2O,  but  gradually  decomp.  when 
in  contact  therewith.  (Meunier,  C.  R.  63. 
330.) 

Caesium,  Cs. 

Decomp.  H2O  with  great  violence.  (Setter- 
berg,  A.  211.  100.) 

Very  sol.  in  liquid  NH3.  (Franklin,  Am. 
Ch.  J.  1898,  20.  827.) 

Caesium  acetylide  acetylene,  Cs2C2,  C2H2. 

Insol.  in  C6H6  and  in  CHC13.  (Moissan, 
C.  R.  1903,  136.  1218.) 

Caesium  amide,  CsNH2. 

Decomp.  by  H2O.  Very  sol.  in  liquid  NH3. 
(Rengade,  C.  R.  1905,  140.  1185.) 


Caesium  cobalt  bromide,  Cs2CoBr4. 

Decomp.  by  H2O.  (Campbell,  Z.  anorg. 
1894,  8.  126.) 

Decomp.  by  H2O  and  by  alcohol.  (Camp- 
bell, Am.  J.  Sci.  1894,  (3)  48.  418.) 

Cs3CoBr5.  Decomp.  by  H2O.  (Campbell, 
Z.  anorg.  1894,  8.  126.) 

Decomp.  by  H2O  and  by  alcohol.  (Camp- 
bell, Am.  J.  Sci.  1894,  (3)  48.  418.) 

Caesium  copper  bromide,  CsBr,  CuBr2. 

Sol.  in  H2O  without  decomp.  (Wells  and 
Walden,  Z.  anorg.  5.  304.) 

2  CsBr,  CuBr2.    (W.  and  W.) 

Caesium  indium  bromide. 
See  Bromiridate,  caesium. 

Caesium  iron  (ferric)  bromide,  CsFeBr4. 

Sol.  in  H2O.  (Walden,  Z.  anorg.  1894,^7. 
332.) 

Cs2FeBr5+H2O.  (Walden,  Z.  anorg.  1894, 
7.  332.) 

Caesium  lead  bromide,  CsBr,  2PbBr2. 

Nearly  stable  in  aqueous  solution.  (Wal- 
den, Sill.  Am.  J.  145.  127.) 

CsBr,  PbBr2.  Decomp.  by  H20.  (Wal- 
den.) 

4CsBr,  PbBr2.    As  above. 

Solubility  determinations  show  that  the 
double  salts  formed  by  csesium  and  lead 
bromides  at  25°  are  CsPb2Br5,  CsPbBr3  and 
Cs4PbBr6.  (Foote,  Am.  Ch.  J.  1907,  37.  125.) 

Caesium  magnesium  bromide,  CsBr,  MgBr2  + 
6H20. 

Sol.  in  H2O.  (Wheeler  and  Campbell,  Z. 
anorg.  5.  275.) 


CASIUM  CHLORIDE 


139 


Caesium  mercuric  bromide,  CsBr,  2HgBr2. 

Not  decomp.  by  H2O.  100  pts.  solution 
sat.  at  16°  contain  0.807  pt.  CsBr,  2HgBr2. 
SI.  sol.  in  hot  strong  alcohol,  from  which 
CsBr,  HgBr2  separates  on  cooling.  (Wells, 
Sill.  Am.  J.  144.  221.) 

CsBr,  HgBr2.  Decomp.  by  H2O  into  above 
salt.  Sol.  in  alcohol  without  decomp.  (Wells.) 

2CsBr,  HgBr2.  Decomp.  by  H2O  into 
CsBr,  2HgBr2. 

3CsBr,  HgBr2.    As  above. 

Caesium  molybdenyl  bromide,  2CsBr, 

MoOBr3. 

(Weinland  and  Knoll,  Z.  anorg.  1905,  44. 
107.) 

Caesium  nickel  bromide,  CsNiBr3. 

Decomp.  by  H2O.    (Campbell,   Z.  anorg. 

1894,  8.  126.) 

Decomp.  by  H2O  and  by  alcohol.  (Camp- 
bell, Am.  J.  Sci.  1894,  (3)  48.  418.) 

Caesium  osmium  bromide. 
See  Bromosmate,  caesium. 

Caesium  palladium  bromide. 

See  Bromopalladate,  caesium  and  bromo- 
palladite,  caesium. 

Caesium  platinum  bromide. 
See  Bromoplatinate,  caesium. 

Caesium  ruthenium  bromide. 
See  Bromoruthenite,  caesium. 

Caesium  selenium  bromide. 
See  Bromoselenate,  caesium. 

Caesium  tellurium  bromide. 
See  Bromotellurate,  caesium. 

Caesium  thallic  bromide,  CsBr,  TlBr3. 

Sol.  in  H2O  with  decomp.    (Pratt,  Z.  anorg. 

1895,  9.  19..) 

By  recryst.  from  H2O,  forms  3CsBr,  2TlBr3. 
(Pratt,  Am.  J.  Sci.  1895,  (3)  49.  403.) 

3CsBr,  2TlBr3.  Can  be  recryst.  unchanged 
from  H2O.  (Pratt,  Am.  J.  Sci.  1895,  (3)  49. 
402.) 

Caesium  tin  (stannic)  bromide. 
See  Bromostannate,  caesium. 

Caesium  zinc  bromide,  3CsBr,  ZnBr2. 

Sol.  in  H2O.  (Wells  and  Campbell,  Z. 
anorg.  5.  275.) 

2CsBr,  ZnBr2.    As  above. 

Caesium    bromide    columbium    oxy bromide, 

2CsBr,  CbOBr3. 

Unstable  in  moist  air.  Decomp.  by  H2O. 
(Weinland,  B.  1906,  39.  3059.) 


Caesium  bromochloride,  CsBr2Cl. 
Properties  as  CsBr3.    (Wells.) 
CsBrCl2.    As  above.    (Wells.) 

Caesium  mercuric  bromochloride, 
Cs3HgCl3Br2. 

Decomp.  by  H2O  finally  to  HgBr2.    (Wells, 
Sill.  Am.  J.  144.  121.) 

Cs2HgCl2Br.    As  above. 

CsHgClBr2.    As  above. 

CsHg2ClBr4.    As  above. 

CsHg5ClBr10.    As  above. 


Caesium  bromochloroiodide,  CsBrClI. 

More  sol.  in  H2O   than  in  alcohol, 
decomp.  at  once  by  ether.    (Wells.) 


Not 


Caesium  bromoiodide,  CsBrI2. 

Decomp.  by  H2O.  Sol.  in  alcohol.  De- 
comp. by  ether  with  residue  of  CsBr.  (Wells, 
Sill.  Am.  J.  143.  17.) 

CsBr2I.  More  sol.  in  H2O  than  in  alcohol. 
Not  decomp.  by  ether. 

CsBr2I+Aq  sat.  at  20°  contains  about 
4.45%CsBr2I.  (Wells.) 

Caesium  carbide,  Cs2C2. 

Decomp.  bv  cold  H2O.  (Moissan,  C.  R. 
1903,  136.  1221.)  • 

Caesium  chloride,  CsCl. 

Very  deliquescent;  sol.  in  H2O  and  alcohol. 

Solubility  of  CsCl  at  t°. 


t° 

Pts.  by  wt.  of  CsCl 
in  100  pts.  solution 

0.3 
10 
20 
30 
40 

61. 
63. 
64. 
66. 
67. 

9 
5 
9 
3 
4 

(Hinrichsen,  Z.  phys.  Ch.  1904, 
Solubility  of  CsCl  at  t°. 

50.  99.) 

t° 

%  CsCl 

t° 

%  CsCl 

0 
10 
20 
30 
40 
50 

61.7 
63.6 
65.1 
66.4 
67.5 
68.0 

60 
70 
80 
90 
100 
119.4 

69.7 
70 
71.4 
72.2 
73.0 
74.4 

(Berkeley,  Trans.  Roy.  Soc.   1904,  203.  A 

A  normal  solution  of  CsCl  has  sp.  gr.  at 
25°  =  1.1076.  (Wagner,  Z.  phys.  Ch.  1890,  5. 

Sp.  gr.  at  20°/4°  of  a  normal  solution  of 
CsCl  =  1.125815.  (Haigh,  J.  Am.  Chem.  Soc. 
1912,  34.  1151.) 


140 


CESIUM  CHROMIUM  CHLORIDE 


Sp.  gr.  of  CsCl+Aq. 

Solubility  of  CsCl+HgCl2  in  acetone  at  25°. 

G.  equiv. 
CsCl  per 
1.  at  18° 

Sp.  gr.                Sp.  gr. 
at  6°/6°           at  18°/18° 

Sp.  gr. 
at  30°/30° 

Solution  contains 

Solid  phase 

%  HgCh 

%  CsCl 

0.504 

1  .  06556        1  .  06483 

1.06452 

57  74 

0.00 

HgCl2 

1.002 
2.007 
3.994 

1  .  12962        1  .  12825 
1.25705        1  25452 
1.50514        1.50100 

1.12750 
1.25307 
1.49859 

57.79 
57.74 
52.54 

0.13 
0.20 
0.22 

HgCl2+CsHg5Cln 

CsHg5Cln 

(Clausen,  W.  Ann.  1914,  (4)  44.  1071.)         49.83 

TCT:  .  O£i  \ 

0.32 
0.501 

u 
CsHg5Cln+CsHg2Cl5 

'  ,    '    ' 

44.46} 

0.44} 

" 

Solubility  of  CsCl+FeCl3  in  H2O  at  21°. 

39.65 

no     A  o 

0.48 

OA  O 

CsHg2Cl5 

Substance  added 

Pts.  by  weight  in  100  pts. 
of  solution 

28.48 
26.96} 

.48 
0.52| 

CsHg2Cl5+CsHgCl3 

07    QO  ! 

0.61  j 

it 

FeCh 
grams 

CsCl 
grams 

FeCb 

CsCl 

—  4    .  •  '  —   j 

21.50 
13.08 

0^46 
0.45 

CsHgCl3 

0 

65 

0 

65.0 

0.16 

0.19 

Mixtures  of  salts 

0.6 

11.6 

0.45 

55.18 

0.17 

0.25 

1  .4 

10.2 

2.  1 

52.38 

0.02 

0.11 

11 

2^2 

8.8 

5.24 

51^44 

0.00 

0.032 

CsCl 

2.0 

3.8 

7.4 
6.0 

7.8 
8.93 

47.70 
41.15 

(Foote  and  Haigh,  J.  Am.  Ch.  Soc.  1911,  33. 
dfii  ^ 

4.6 

4.6 

15.34 

25.25 

5.4 

2  8 

21  .65 

14.96 

6^2 

^  .  O 

1.4 

27*96 

8^42 

Insol. 

in  methyl  acetate.     (Naumann,  B. 

35 
35 

0.2 
0 

48.71 
83.89 

0.94 
0 

1909,  42.  3790.) 
Solubility  in  glycol  at  ord.  temp.  =  10.6- 

10  8%       (dp  Doninr>lt.  Rplff    Arsfld    Rnll    1905. 

(Hinrichsen,  Z.  phys.  Ch.  1904,  60.  96.) 

359.) 

. 

Insol. 

in  anhydrous  pyridine  and  in  97% 

Solubility  of  CsCl+HgCl2  in  H2O  at  25°. 

pyridine+Aq.     SI.  sol.  in  95%  pyridine+Aq 
and  in  93%  pyridine+Aq.     (Kahlenberg,  J. 

Solution  contains 

Am.  Chem.  Soc.  1908,  30.  1107.) 

Q        I-     1               1 

%  CsCl 

%  HgCl-2 

Caesium  chromium  chloride,  2CsCl,CrCl3  + 

65.61 
65.78 
62.36 
57.01 
52.35 

0.00 
0.215 
0.32 
0.64 
1.23 

CsCl 
CsCl+Cs3HgCl5 
Cs3HgCl5 

u 

H2O. 
Stable  in  the  air.    Sol.  in  H2O.    (Wells,  Z. 
anorg.  1895,  10.  182.) 
2CsCl,CrCl3+4H2O;  hydroscopic;  very  sol. 
in  H2O.    (Wells,  I.  c.) 

51.08 
49.30 
45  95 

1.44 
1.49 
1  69 

Cs3HgCl5+Cs2HgCl4 
Cs2HgCl4 

Caesium  tetra-aquochiomium  chloride, 
CrCl2(OH2)4.Cl,  2CsCl. 

45.23 

1.73 

Cs2HgCl4+CsHgCl3 

Ppt. 

(Werner,  B.  1901,  34.  1602.) 

38.63 
17.03 

1.32 
0.51 

CsHgCl3 

Caesium  cobalt  chloride,  CsCoCl3+2H2O. 

1.53         0.42 

" 

Decomp.  by  H2O  and  alcohol.    (Campbell, 

0.61 

2.64 

CsHgCl3+CsHg2Cl5 

Z.  anorg.  1894,  8.  126.) 

0.49 

2.91 

CsHg2Cl5 

Cs2CoCl4.     Decomp.  by  H2O  and  by  al- 

0.40 

3.78 

CsHg.CU+CsHgsCln 

cohol. 

(Campbell,  Z.  anorg.  1894,  8.  126.) 

0.44 

4.63 

u 

Cs3CoCl5.     Decomp.  by  H2O  and  by  al- 

0.41 
0.25 

4.68 
5.65 

CsHg5Clu 

cohol. 

(Campbell,  Z.  anorg.  1894,  8.  126.) 

0.18 

7.09 

CsHg5Cln+HgCl2 

Caesium  cuprous  chloride,  CsCl,  Cu2Cl2. 

0.00 

6.90 

HgCl2 

Decomp.  by  H2O  into  CuCl2,  CsCl.  (Wells, 

(Foote,  Am.  Ch.  J.  1903,  30.  340.) 

Z.  anorg.  5.  306.) 
3CsCl,  Cu2Cl2.    (Wells.) 

6CsCl,  Cu2Cl2.    (Wells.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

100  g.  solution  in  acetone  sat.  at  25°  con- 
tain 0.032  g.  CsCl.  (Foote  and  Haigh,  J. 
Am.  Chem.  Soc.  1911,  33.  461.) 


Caesium  cupric  chloride,  2CsCl,  CuCl2. 

Easily   sol.    in    H2O    and    dil.    HCl+Aq; 
insol.    in    cone.    HCl+Aq.      (Godeffroy,    B. 


CASIUM  SAMARIUM  CHLORIDE 


141 


Sol.  in  small  amount  H2O  without  decomp. 
(Wells  and  Dupee,  Z.  anorg.  6.  300.) 

+2H2O.    Efflorescent.    (W.  and  D.) 

3CsCl,  2CuCl2+2H2O. 

CsCl,  CuCl2.  Sol.  in  H2O  without  decomp. 
(W.  and  D.) 

Caesium  gold  chloride. 
See  Chloraurate,  caesium. 


Caesium  indium 
See  Chloriridate,  caesium. 

Caesium    iron    (ferric)    chloride,    CsFeCl4 


Sol.  in  H2O.  Decomp.  in  the  air.  (Wai- 
den,  Z.  anorg.  1894,  7.  332.)  <•*» 

Cs2FeCl5+H2O.     Sol.  in  H2O.     (Walden.) 
Cs3FeCl6+H2O.    Sol.  in  H2O.    (Walden.) 

Caesium     lanthanum     chloride,    Cs3LaCl6  + 

4H2O. 

Very  hydroscopic.  Easily  sol.  in  H2O. 
(R.  J.  Meyer,  Z.  anorg.  1914,  86.  273.) 

Caesium  lead  chloride,  CsCl,  2PbCl2. 

Nearly  stable  in  aqueous  solution.  (Camp- 
bell, Sill.  Am.  J.  145.  126.) 

CsCl,  PbCl2.  Decomp.  by  H2O.  (Camp- 
bell.) 

4CsCl,  PbCl2.    As  above.    (Campbell.) 

Caesium  lead  te/rachloride. 
See  Chloroplumbate,  caesium. 

Caesium  magnesium  chloride,  CsCl,  MgCl2  + 

6H2O. 

Sol.   in   H20. 
anorg.  5.  275.) 

Caesium  manganous  chloride,  CsCl,  MnCl2  + 
2H2O. 

Not  deliquescent;  sol.  in  H2O.  (Saunders, 
Am.  Ch.  J.  14.  143.) 

2CsCl,  MnCl2.    (Godeffroy.) 

+2^H20.     (Godeffroy.) 

+3H2O.  Sol.  in  H2O.  Cone.  HCl+Aq 
precipitates  anhydrous  salt  from  aqueous 
solution.  (Godeffroy,  B.  8.  9.) 

The  only  salt  which  exists  contains  2H2O. 
(Saunders,  Am.  Ch.  J.  14.  143.) 

Caesium  manganic  chloride,  2CsCl,  MnCls. 

Easily  decomp.  (Meyer  and  Best,  Z 
anorg.  1899,  22.  187.) 


(Wells   and   Campbell,   Z. 


Caesium  mercuric  chloride,  CsCl,  HgCl2. 

100  pts.  solution  sat.  at  17°  contain  1.406 
pts.  CsHgCl3.  Not  decomp.  by  H2O.  Insol 
in  absolute  alcohol,  but  sol.  on  diluting  witt 
Va  vol.  H2O.  (Wells,  Sill.  Am.  J.  144.  221.) 

2CsCl,  HgCl2.  Easily  sol.  in  H2O  and  dil 
HCl+Aq;  insol.  in  cone.  HCl+Aq.  (Godef- 
froy.) 


3CsCl,  HgCl2.  Decomp.  by  HoO;  on  re- 
crystallizing  from  H2O,  CsCl,  HgCl2  is  finally 
formed.  (Wells,  Sill.  Am.  J.  144.  221.) 

CsCl,  5HgCl2.  Decomp.  by  H2O.  (Wells.) 
Solubility  determinations  show  that  the 
only  double  salts  of  CsCl  and  HgCl2  which 
exist  at  25°  are  Cs3HgCl5,  Cs2HgCl4,  CsHgCl3, 
CsHg2Cl5,  CsHg5Cln.  (Foote,  Am.  Ch.  J. 
1903,  30.  340.) 

Caesium  molybdenum  chloride,  Cs2MoCl5  + 

.  H2G. 

Sol.  in  H2O.  Nearly  insol.  in  alcohol  and 
ether.  (Chilesotti,  C.  C.  1903,  II.  652.) 

Caesium  molybdenyl  chloride,   CsCl, 
MoO2Cl2+H2O. 

Hygroscopic.  Decomp.  by  H2O.  (Wein- 
and  and  Knoll,  Z.  anorg.  1905,  44.  93.) 

2CsCl,  MoO2Cl2.  Hygroscopic.  Decomp. 
3y  H2O.  (Weinland  and  KnoH,  Z.  anorg. 
1905,  44.  92.) 

2CsCl,  6MoO2Cl2+22H2O.  Very  hygro- 
scopic. Decomp.  by  H2O.  (Weinland  and 
Knoll,  Z.  anorg.  1905,  44.  94.) 

2CsCl,  MoOCl3.  Only  si.  sol.  in  H2O. 
:Nordenskjold,  B.  1901,  34.  1573.) 

Caesium    neodymium    chloride,    Cs3NdCl6  + 

5H2O. 

Very  hydroscopic.  Easily  sol.  in  H2O. 
R.  J.  Meyer,  Z.  anorg.  1914,  86.  273.) 

;sesium  nickel  chloride,  2CsCl,  NiCl2. 

As  the  corresponding  Cu  salt. 

CsNiCl3.  Decomp.  by  H2O  and  by  alcohol. 
(Campbell,  Am.  J.  Sci.  1894,  (3)  48.  418.) 

Caesium  palladium  ^chloride. 
See  Chloropallad;te,  caesium. 

Caesium  palladium  /drachloride. 
See  Chloropalladate,  caesium. 

Caesium  praseodymium  chloride,  Cs3PrCl6  + 

5H20. 

Very  hydroscopic.  Easily  sol.  in  H2O. 
(R.  J.  Meyer,  Z.  anorg.  1914,  86.  273.) 

Caesium  rhodium  chloride. 
See  Chlororhodite,  caesium. 

Caesium  ruthenium  chloride. 

See  Chlororuthenite,  caesium  and  chloro- 
ruthenate,  caesium. 

Caesium  oa:?/ruthenium  chloride, 

Cs2RuO2Cl4. 

Ppt.:  decomp.  by  H2O;  sol.  in  cold  HC1. 
(Howe,  J.  Am.  Chem.  Soc.  1901,  23.  779.) 

Caesium     samarium     chloride,     Cs3SmCl6+ 

5H20. 

Very  hydroscopic.  Easily  sol.  in  H2O. 
(R.  J.  Meyer,  Z.  anorg.  1914,  86.  273.) 


142 


OfcSIUM  SILVER  CHLORIDE 


Caesium  silver  chloride,  2CsCl,  AgCl. 

Easily  decomp.  by  H2O.  (Wells  and 
Wheeler,  Sill.  Am.  J.  144.  155.) 

Caesium  tellurium  chloride. 
See  Chlorotellurate,  caesium. 

Caesium  thallic  chloride,  2CsCl,  T1C13. 

By  recryst.  from  H2O  forms  3CsCl,  2T1C13. 
(Pratt,  Am.  J.  Sci.  1895,  (3)  49.  398.) 

+H2O.  Readily  sol.  in  hot  H2O  but  SCsCl, 
2T1C13  cryst.  from  the  solution.  (Pratt,  Am. 
J.  Sci.  1895,  (3)  49.  399.) 

SCsCl,  2T1C13.  Can  be  recryst.  from  H2O 
without  change.  (Pratt,  Am.  J.  Sci.  1895,  (3) 
49.  401.) 

3CsCl,  T1C13+2H2O.  Sol.  in  36.4  pts.  H2O 
at  17°  and  3  pts.  at  100°.  (Godeffroy,  Zeitsch. 
d.  allgem.  osterr.  Apothekerv.  1880.  No.  9.) 

Caesium  tin  (stannic)  chloride. 
See  Chlorostannate,  caesium. 

Caesium  titanium  chloride,  TiCl3,   2CsCl  + 

H20. 

Difficultly  sol.  in  H2O.  (Stabler,  B.  1904, 
37.  4409.) 


Caesium  tungsten  chloride,  Cs3W2Cl9. 

Nearly  insol.  in  cold  H2O. 

Sol.  in  a  hot  mixture  of  equal  pts.  H2O  and 
cone.  HC1. 

Nearly  insol.  in  cone.  HC1. 

Sol.  in  very  dil.  NaOH+Aq. 

Nearly  insol.  in  most  organic  solvents. 
(Olsson,  B.  1913,  46.  574.) 

Caesium  uranous  chloride,  Cs2UCl6. 

As  K  salt.  (Aloy,  Bull.  Soc.  1899,  (3)  21. 
264.) 

Caesium  uranyl  chloride,  2CsCl,  (UO2)C12. 

Sol.  in  H2O.  (Wells,  Z.  anorg.  1895,  10. 
183.) 

100  pts.  of  the  solution  contain  at  29.75°, 
56.07  pts.  UO2C12,  2CsCl.  (Rimbach,  B. 
1904,  37.  468.) 

Pptd.  from  aq.  solution  by  gaseous  HC1. 
(Wells,  Am.  J.  Sci.  1894,  (3)  60.  251.) 

Caesium  vanadium  chloride,  Cs2VdCl5+H2O. 
Difficultly  sol.  in  H2O  and  alcohol.    (Stab- 
ler, B.  1904,  37.  4412.) 

Caesium  zinc  chloride,  SCsCl,  ZnCl2. 

Sol.  in  H2O.  (Wells  and  Campbell,  Z. 
anorg.  6.  275.) 

2CsCl,  ZnCl2.  Easily  sol.  in  HoO  and  dil. 
HCl+Aq.  Insol.  in  cone.  HCl+Aq.  (Godef- 
froy.) 


Caesium  chloride  chromic  oxychloride, 
2CsCl,  CrOCl3. 

Decomp.  in  the  air. 

Sol.  in  cone.  HC1  without  decomp.  (Wein- 
land,  B.  1906,  39.  4045.) 

Caesium    chloride    columbium    oxychloride, 

2CsCl,  CbOCl3. 

Decomp.  by  H2O.  (Weinland,  B.  1906, 
39.  3057.) 

Caesium  chloroiodide,  CsCl2I. 
Properties  as  CsBrClI.    (Wells.) 
CsClJ.    Si.  sol.  in  H2O,  from  which  it  can 

be  recrystallized   without   decomp.      (Wells 

and  Wheeler.) 

Caesium  mercuric  chloroiodide,  Cs2HgCl2I2. 
Decomp.  instantly  by  H2O  to  HgI2.  (Wells.) 

Caesium  fluoride,  CsF. 

Ppt.    (Chabrie,  C.  R.  1901,  132.  680.) 
+1^H20.  100  g.  H2O  dissolve  366.5  g  CsF 

at  15°.  (de  Forcrand,  C.  R.  1911,  162.  1210.) 

Caesium  hydrogen  fluoride,  CsHF2. 
Ppt.    (Chabrie,  C.  R.  1901,  132.  680.) 

Caesium  tantalum  fluoride. 
See  Fluotantalate,  caesium. 

Caesium  tellurium  fluoride,  CsF,TeF4. 

Decomp.  by  H2O.  (Wells,  Am.  J.  Sci.  1901, 
(4)  12.  190.) 

Caesium  titanium  fluoride. 
See  Fluotitanate,  caesium. 

Caesium  zirconium  fluoride. 
See  Fluozirconate,  caesium. 

Caesium  hydride,  CsH. 

Decomp.  by  H2O  with  evolution  of  H2. 
(Moissan,  C.  R.  1903,  136.  589.) 

Caesium  hydroxide,  CsOH. 

Very  deliquescent,  and  sol.  in  H2O.  Sol. 
in  alcohol. 

79.41%  CsOH  is  contained  in  a  sat.  aq.  solu- 
tion at  15°.  (de  Forcrand,  C.  R.  1909,  149. 
1344.) 

75.08%  CsOH  is  contained  in  sat.  aq.  solu- 
tion at  30°.  (Schreinemakers,  C.  C.  1909,  I. 
11.) 

Caesium  iodide,  Csl. 

Sol.  in  H2O. 

100  pts.  H2O  dissolve  44  pts.  Csl  at  0°; 
66.3  pts.  at  14.5°;  160  pts.  at  61°. 

Sp.  gr.  of  CsI+Aq  sat.  at  14°  =  1.393. 
(Betekoff,  Bull.  Soc.  Petersb.  (4)  2.  197.) 


CALCIUM  AMALGAM 


143 


Caesium  periodide. 

Solubility  determinations  show  that  CsI3 
and  Csls  are  the  only  periodides  of  caesium 
existing  between  — 4°  and  +73°.  (Foote, 
Am.  Ch.  J.  1903,  29.  203.) 

Caesium  fniodide,  CsI3. 


1  com.  sat.  CsI+Aq  dissolves  0.0097  g. 
CsI3,  and  sp.  gr.  of  solution  is  1.154.  Only  si. 
decomp.  by  solution  in  H2O.  Much  more 
sol.  in  alcohol  than  in  H2O.  Not  immediately 
decomp.  by  ether.  (Wells,  Sill.  Am.  J.  143. 
17.) 

Caesium  pentaiodide,  Csls. 

Caesium  cobalt  iodide,  Cs2CoI4. 

Decomp.  by  H2O.     (Campbell,  Z.  anorg. 

1894,  8.  12.) 

Deliquescent;  decomp.  by  H2O  and  by 
alcohol.  (Campbell,  Am.  J.  Sci.  1894,  (3) 
48.  418.) 

Caesium  lead  iodide,  CsPbI2. 

SI.  sol.  in  hot  Csl -f  Aq.  (Wheeler,  Sill.  Am. 
J.  145.  129.) 

Caesium  mercuric  iodide,  Csl,  2HgI2. 

Decomp.  by  H2O  finally  into  HgI2.  (Wells, 
Sill.  Am.  J.  144.  221.) 

2CsI,  3HgI2.  Decomp.  by  H2O  finally  into 
Hgl*. 

Csl,  HgI2.    As  above. 

2CsI,  HgI2.  Decomp.  by  H2O;  insol.  in 
alcohol. 

3CsI,  HgI2.    As  above. 

Caesium  silver  iodide,  Csl,  Agl. 

(Penfield,  Z.  anorg.  1.  100.) 

Csl,  2AgI.  More  sol.  in  hot  than  in  cold 
acetone.  (Marsh,  Chem.  Soc.  1913,  103. 

782.) 

Caesium  tellurium  iodide. 
See  lodotellurate,  caesium. 

Caesium  thallic  iodide,  Csl,  T1I3. 

Decomp.   by  H2O.      (Pratt,   Am.   J.    Sci. 

1895,  (3)  49.  403.) 

Caesium  zinc  iodide,  3CsI,  ZnI2. 

Sol.  in  H2O.  (Wells  and  Campbell,  Z. 
anorg.  5.  275.) 

2CsI,  ZnI2.    As  above. 

Caesium  oxide,  Cs2O. 

Absorbs  H2O  and  CO2  from  the  air. 
Decomp.  by  H2O  and  by  liquid  NH3.  (Ren- 
gade,  C.  R.  1906,  143.  593.) 

Caesium  dioxide,  Cs2O2. 

Decomp.  by  H2O.  (Rengade,  C.  R.  1905, 
140.  1537.) 


Caesium  In'oxide,  Cs2Os. 

Decomp.  by  H2O.  (Rengade,  C.  R.  1905, 
140.  1537.) 

Caesium  tefroxide,  Cs2O4. 

Decomp.  by  H2O.  (Rengade,  C.  R.  1905, 
140.  1538.) 

Caesium  sulphide,  Cs2S+4H2O. 

Deliquescent;  very  sol.  in  H2O.  (Biltz, 
Z.  anorg.  1906,  48.  300.) 

Caesium  bisulphide,  Cs2S2. 

Anhydrous.  Sol.  in  H2O.  Hydroscopic. 
(Biltz,  Z.  anorg.  1906,  60.  72.) 

+H2O.  From  Cs2S2+Aq.  Hydroscopic. 
(Biltz,  Z.  anorg.  1906,  50.  72.) 

Caesium  /nsulphide,  Cs2S3. 

Anhydrous.  Sol.  in  H2O.  Not  hydroscopic. 
(Biltz,  Z.  anorg.  1906,  50.  75.) 

+H2O.  From  Cs2S3+Aq.  (Biltz,  Z. 
anorg.  1906,  50.  76.) 

Caesium  te^rasulphide,  Cs2S4. 

Sol.  in  H2O.  Insol.  in  abs.  alcohol.  (Biltz, 
Z.  anorg.  1906,  48.  305.) 

Caesium  perctasulphide,  Cs2S6. 

Mpt.  2°.  Not  hydroscopic.  Very  sol.  in 
cold  70%  alcohol.  (Biltz,  B.  1905,  38.  129.) 

Caesium  hydrogen  sulphide,  CsHS. 

Deliquescent;  very  sol.  in  H2O.  (Biltz, 
Z.  anorg.  1906,  48.  300.) 

Caesium  copper  tefrasulphide,  CsCuS4. 

SI.  sol.  in  cold  H2O. 

Decomp.  by  cone,  and  dil.  HC1,  H2SO4  and 
HNO3. 

SI.  sol.  in  alcohol.    (Biltz,  B.  1907,  40.  978.) 

Calcium,  Ca, 

Decomp.  H2O  violently.  Slowly  attacked 
by  cold  H2S04.  Dil.  H2S04+Aq  or  HCl+Aq 
attack  violently  and  dissolve.  Dil.  HNO3  + 
Aq  oxidizes,  but  fuming  HNO3  scarcely  at- 
tacks even  on  boiling.  (Bunsen  and  Matthies- 
sen  )  Not  attacked  by  anhydrous  alcohol. 
(Lies-Bodart  and  Jobin,  A.  ch.  (3)  54.  364.) 

Pure  Ca  is  only  very  slowly  decomp.  by 
H2O  at  ordinary  temp.;  sol.  in  HC1,  HNO3, 
H2SO4.  (Moissan,  C.  R.  1898,  129.  589.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  827.) 

YL  com.  oleic  acid  dissolves  0.0334  g.  Ca 
in  6  days.  (Gates,  J.  phys.  Chem.  1911,  15. 
143.) 

Calcium  amalgam,  Ca3Hg4. 

Decomp.  H2O  readily.  (Fere,  C.  R.  1898, 
127.  619.) 

CaHg5.  Rapidly  decomp.  in  moist  air. 
(Schiirger,  Z.  anorg.  1900,  25.  425.) 


144 


CALCIUM  AMIDE 


Calcium  amide,  Ca(NH2)2. 

(Moissan,  A.  ch.  1899,  (7)  18.  326.) 

Calcium  ammonia,  Ca,  4NH3. 

Decomp.  at  ordinary  temp.;  takes  fire  in 
contact  with  the  air;  si.  sol.  in  liquid  NH3. 
(Moissan,  C.  R.  1898,  127.  691.) 

Ca,6NH3.  (Kraus,  J.  Am.  Chem.  Soc. 
1908,  30.  665.) 

Calcium  arsenide,  Ca3As2. 

Decomp.  by  cold  H2O;  insol.  in  cold  fuming 
HNO3;  very  sol.  in  hot  HNO3.  (Lebeau, 
C.  R.  1899,  128.  98.) 

Calcium  azoimide,  Ca(N3)2. 

Hydroscopic;  explosive. 
38.1     pts.  sol.  in  100  pts.       H2O        at    0° 

45.0  "     "      "  100    "          H2O         "  15.2 
0.211   "     "      "  100    "    abs.  alcohol  "  16. 

Sol.  in  H2O;  decomp.  when  heated  and  on 
standing  in  the  air.  (Dennis,  Z.  anorg.  1898, 
17.  21.) 

Insol.  in  pure  ether.  (Curtius,  J.  pr.  1898, 
(2)  68.  286.) 

Calcium  boride,  CaB6. 

Not  decomp.  by  H2O  at  250°;  sol.  in  fused 
oxidizing  agents. 

Insol.  in  aq.  acids;  si.  sol.  in  cone.  H2SO4; 
sol.  in  dil.  or  cone.  HNO3.  (Moissan,  C.  R. 
1897,  125.  631-32.) 

Calcium  bromide,  CaBr2. 

Very  deliquescent.  100  pts.  H2O  dissolve — 
at  0°  20°  40C  60C  105° 

125      143      213     -278      312  pts.  CaBr2. 
(Kremers,  Pogg.  103.  65.) 

Sat.  CaBro+Aq  contains  at: 
—22°     —22°     —14°      —7°       — 5C 
50.5      50.2      52.5      52.6      52.6%  CaBr2 

+8°       9°  11°        20°         50° 

53.1  55.1      55.7      57.1       62.6%  CaBr2 
(fitard,  A.  ch.  1894,  (7)  2.  540.) 

Sp.  gr.  of  CaBr2+Aq  at  19.5°  containing: 
5  10          15          20         25  %CaBr2, 

1.044     1.089     1.139     1.194    1.25? 

30          35          40         45         50  %  CaBr2. 
1.315     1.385     1.461     1.549     1.641 
(Kremers,  Pogg.  99.  444,  calculated  by  Ger- 
lach,  Z.  anal.  8.  285.) 

SI.  sol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Very  sol.  in  alcohol.    (Henry.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899,  II. 
1014;  Naumann,  B.  1904,  37.  4328.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 


Sol.  in  ethyl  acetate.  (Naumann,  B.  1910, 
43.  314.) 

Insol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1370.) 

+4H2O.     (Kuznetzov,  C.  A.  1911.  842.) 

+6H2O. 

Calcium   manganous    bromide,    GaMnBr4  + 

4H2O. 

SI.  hydroscopic.  Unstable.  (Ephraim,  Z. 
anorg.  1910,  67.  377.) 

Calcium  mercuric  bromide. 

Decomp.  by  H2O.    (v.  Bonsdorff.) 

Calcium  molybdenyl  bromide,  CaBr2, 

2MoOBr3+7H2O. 

(Weinland  and  Knoll,  Z.  anorg.  1905,  44. 
112.) 

Calcium  stannic  bromide. 
See  Bromostannate,  calcium. 

Calcium  bromide  ammonia,  CaBr2,  6NH3. 
Sol.  in  H2O.   (Rammelsberg,  Pogg.  56.  239.) 

Calcium  bromide  hydrazine,  CaBr2,  3N2H4. 

Easily  sol.  in  H2O.  (Franzen,  Z.  anorg. 
1908,  60.  288.) 

Calcium  bromofluoride,  CaBr2,  CaF2. 

Decomp.  by  H2O.  (Defacqz,  A.  ch.  1904, 
(8)  1.  357.) 

Calcium  carbide,  CaC2. 

Sp.  gr.  2.22  at  18°.  Insol.  in  fuming  HNO3 
and  cone.  H2SO4  but  readily  decomp.  by 
dil.  acids  and  H2O.  (Moissan,  Bull.  Soc. 
1894,  (3)  11.  1005.) 

Insol.  in  HC1  in  the  cold,  but  decomp.  at 
red  heat.  Strong  min.  acids  do  not  act  in 
the  cold;  sol.  in  glacial  acetic  in  the  cold; 
sol.  in  fused  alkali.  (Venable,  J.  Am.  Chem. 
Soc.  1895,  17.  307-310.) 

Calcium  chloride,  CaCl2. 

Very  deliquescent.  Veiy  sol.  in  H2O  with 
evolution  of  heat. 

Anhydrous  CaCh  is  sol.  in  1.459  pts.  H2O.    (Gerlach.) 

Anhydrous  CaCl2  is  sol.  in  1.58  pts.  H2O  at  10.2°. 
(Kremers,  Pogg.  103.  65.)  - 

Anhydrous  CaCh  is  sol.  in  1.35  pts.  H2O  at  20°;  O.S3 
pt.  H20  at  40°;  0.72  pt.  H2O  at  60°.  CaCh+6HsO  is 
sol.  in  0.5  pt.  H2O  at  0°,  and  2.05  pt.  at  16°.  (Gmelin.) 

CaCl2  is  sol.  in  1.5  pts.  cold,  and  0.8  pt.  boiling  H2O. 
(Fourcroy.) 

CaClz+Aq  sat.  in  the  cold  contains  40.7%  CaCK>. 
(Fourcroy.) 

CaCl2+Aq  sat.  at  12.5°  contains  53.8%  CaCl2. 
(Hassenfratz.) 

100  pts.  H2O  dissolve  165.7  pts.  CaCl2  + 
6H2O  at  0°;  7141  pts.  at  40°.  (Tilden,  Chem. 
Soc.  45.  409.) 

100  pts.  H2O  dissolve  60.3  pts.  CaCl2  from 
CaCl2+6H2O  at  0°,  and  solution  has  sp.  gr.  = 
1.367.  (Engel,  Bull.  Soc.  (2)  47.  318.) 


CALCIUM  CHLORIDE 


145 


Solubility  of  CaCl2+6H2O  in  H2O  at  t°. 

If  so 
100  pts 
to  +6° 
(Etard, 
Acco] 
bility  oi 
employ 
tained  £ 

Solubili 

[ubility  S=pts.  anhydrous  C 
.  solution,  S  =  32+0.2148t  fron 
;  S  =  54.5+0.0755t  from  50°  t 
C.  R.  98.  1432.) 
•ding  to  Bakhuis  Roozeboom,  t 
CaCl2  varies  according  to  the  ] 
3d,  and  the  following  data  w 
is  the  result  of  very  exact  exper 

ty  of  CaCl2+6H2O  in  100  pt 
at  t°. 

aC!2  in 

t 

Sat.    solution 
contains 
%  CaCh 

Sat.  solution 
contains 
%CaCh+6H20 

i  —  18 
o  120°. 

le  solu- 
lydrate 
ere  ob- 
iments. 

s.  H20 

—22 
0 
+  7.39 
13.86 
19.35 
23.46 
24.47 
27.71 
29.53 

32.24 
36.91  ' 
38.77 
41.03 
42.50 
44.15 
45.33 
46.30 
50.67 

63.61 
72.82 
76.49 
80.95 
83.85 
87.11 
89.44 
91.35 
99.97 

t° 

Pts. 
CaCh 

t° 

Pts. 
CaCh 

t° 

Pts. 
CaCh 

(Hammerl,  W.A.B.  72,  2.  287.) 
Solubility  in  100  pts.  H2O  at  t°. 

20.4 
25.05 

75.1 

81.67 

28.0 
28.9 

88.8 
92.05 

29.5 
30.2 

96.07 
102.7 

t°              Pts.  CaCh 

t°                Pts.  CaC  h 

There  are  two  modifications  of  CaCl2  + 
4H2O,  a  and/3. 

Solubility  of  CaCl2H-4H2O|8  in  100  pts. 
H2O  at  t°. 

0                59.39 
5                64.83 
7.88           66.20 

13.86         69.49 
19.35         73.91 
21.89         79.77 

(Hammerl,    calculated     by    Bakhuis   Rooze 
boom,  R.  t.  c.  8.  5.) 

Solubility  in  100  pts.  H2O  at  t°. 

t 

Pts.  CaCh 

t°              Pts. 

CaCh 

t 

Pts. 
CaCh 

t° 

Pts. 
CaCh 

t° 

Pts. 
CaCh 

18.4 
25  0 
30.0 

103  3 
108.8 
114.1 

35.0           122.74 
38.4           127.50 

0 
1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
57 
58 
59 
60 
61 
62 
63 
64 
65 
66 
67 
68 
69 
70 
71 

49.6 
50 
51 
52 
53 
54 
55 
56 
57 
58 
60 
61 
62 
63 
65 
66 
68 
69 
71 
127 
128 
129 
129 
130 
131 
131 
132 
133 
133 
134 
135 
135 
136 
136 

19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
34 
35 
36 
37 
72 
73 
74 
75 
76 
77 
78 
79 
80 
81 
82 
83 
84 
85 
86 

72 

74 
75 
77 
79 
80 
82 
84 
87 
89 
91 
93 
96 
98 
100 
103 
104 
105 
107 
137 
138 
138 
139 
139 
140 
141 
141 
142 
142 
143 
143 
144 
144 
145 

38 
39 
40 
41 
'42 
43 
44 
45 
46 
47 
48 
49 
50 
51 
52 
53 
54 
55 
56 
87 
88 
89 
90 
91 
92 
93 
94 
95 
96 
97 
98 
99 
179.5 

108 
109 
110 
111 
112 
113 
114 
115 
116 
117 
118 
119 
120 
121 
122 
123 
124 
125 
126 
145 
146 
147 
147 
148 
149 
150 
150 
151 
152 
152 
153 
154 
325 

Solubility  of  CaCl2+4H2Oa  in  100  pts.  H2O 
att°. 

t° 

22.0 

24  7 
29  8 

Pts.  CaCh 

t° 

Pts.  CaCh 

92  67 
95.59 
100.6 

35.95 
40.00 
45.00 

107.21 
115  3 
129.9 

Solubility  of  CaCl2+2H2O  in  100  pts.  H2O 
att°. 

t° 

Pts. 

CaCh 

t° 

Pts. 
CaCh 

t° 

Pts. 
CaCh 

40 
45 
50         1 
59.5     1 
80.5     ] 

[28.1 
[29.9 
[32.3 
[36.5 
[45.3 

95.8 
115 
124 
137 

156.5 
169.5 
176.0 
187.6 

139 
155 
165 
174 

191.0 

214.3 
236.2 
275.7 

Solubility  of  CaCl2+H2O  in  100  pt 
at  t°. 

s.  H2O 

t° 

Pts.  CaCh 

191 
235 

306 
331 

(Mulder,  Scheik.  Verhandel.  1864.  107.) 

(Bakhuis  Roozeboom,  R.  t.  c.  8.1.) 

146 


CALCIUM  CHLORIDE 


Sp.  gr.  of  CaCl2+Aq. 


CaCl2 

Sp.  gr. 

c?h, 

Sp.  gr. 

% 
CaCh 

Sp.  gr. 

3.95 
7.66 
11.23 
14.42 
17.60 

1.03 
1.06 
1.09 
1.12 
1.15 

20.85 
23.93 
26.86 
29.67 
32.35 

.18 
.21 
.24 
.27 
.30 

34.57 
36.49 
38.31 
40.43 
41.91 

1  .  33 
1.36 
1.39 
1.42 
1.45 

(Richter.) 


Sp.  gr.  of  CaCU+Aq  at  19.5°  containing  pts.  CaCl2  to 
100  pts.  H2O. 


Pts. 
CaCh 

Sp.  gr. 

Pts. 
CaCl2 

Sp.  gr. 

6.97 
12.58 
23.33 

1.0545 
1.0954 
1  .  1681 

36.33 
50.67 
62.90 

1  .  2469 
1.3234 
1  .  3806 

(Kremers,  Pogg.  99.  444.) 


Sp.  gr.  of  CaCl2+Aq.  G  =  sp.  gr.  at  15°  if  % 
is  CaCl2,  according  to  Gerlach;  S  =  sp.  gr. 
at  18.3°  if  %  is  CaCl2-f6H2O,  according 
to  Schiff. 


Sp.  gr.  of  CaCl2+Aq  :  a  =  nb.  of  half  molecules 
in  grammes  dissolved  in  1000  g.  H2O; 
b  =  sp.  gr.  at  24.3°  when  a  =  CaC!2  + 
6H2O  (Y2  mol.  =  109.5  g.);  c  =  sp.  gr.  at 
24.3°  when  a  =  CaC!2  (^  mol.=55.5  g.). 


a 

b 

c 

a  ' 

b 

o 

1 

2 
3 
4 
5 
6 

.041 
.076 
.106 
.133 
.157 
1  .  179 

1.043 
1.084 
1.122 
1.159 
1.193 
1  227 

7 
8 
9 
10 
11 

1.198 
1.214 
1.229 
1.242 
1.255 

1.25S 

(Favre  and  Valson,  C.  R.  79.  968.) 


Sp.  gr.  of  CaCl2+Aq  at  18°. 


%  CaCl2 


5 
10 
15 
20 


Sp.  gr. 


1 . 0409 
1.0852 
1.1311 
1 . 1794 


%  CaCl2 


25 
30 
35 


Sp.  gr. 


1.2305 
1.2841 
1.3420 


3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
34 
35 


G 


.00852 
.01704 
.02555 
.03407 
. 04259 
.05146 
.06033 
.06921 
.07808 
.08695 
.09628 
.00561 
. 10494 
. 12427 
. 13360 
. 14332 
. 15305 
. 16277 
. 17250 
. 18222 
. 19251 
. 20279 
.21308 
.22336 
.23365 
. 24450 
.25535 
.26619 
.27704 

28789 
.29917 
.31045 
. 32174 
.33602 

34430 


8 


1.0039 
1.0079 
1.0119 
1.0159 
1.0200 
1.0241 
1.0282 
1.0323 
1.0365 


0407 

0449 

0491 

0534 

0577 

0619 

0663 

1.0706 

1.0750 

1.0794 

1.0838 

1.0882 

1  0927 

0972 

1017 

1062 

1107 

1153 

1199 

1246 

1292 

1339 

1386 


1.1433 
1.1480 
1 . 1527 


35610 
36790 
37970 
39150 
40330 


1 . 1575 
.1622 
.1671 
.1719 
.1768 
.1816 
.1865 
.1914 
.1963 
.2012 
.2062 
.2112 
.2162 
.2212 
.2262 
.2312 
.2363 
.2414 
.2465 
.2516 
.2567 
.2618 
.2669 
.2721 
.2773 
.2825 
.2877 
.2929 
.2981 
.3034 
.3087 
.3140 
.3193 
.3246 
.3300 


(Kohlrausch,  W.  Ann.  1879.  1.) 


CaCl2+Aq  sat.  at  0°  has  sp.  gr.  =  1.367. 
(Engel,  Bull.  Soc.  1887,  (2)  47.  318.) 


Sp.  gr.  of  CaCl2+Aq  at  9.5°C. 


Mass  of  salt  per  unit 
mass  of  solution 


0.00191 
0.00381 
0.00570 
0.00759 
0.00947 
0.01320 


Density  of  solution 
(g.  per  cc.) 


1.00168 
1.00317 
1 . 00465 
1.00615 
1.00765 
1.01050 


(McGregor,  C.  N.  1887,  55.  6.) 


Sp.  gr.  of  CaCl2+Aq  at  25°. 


Concentration  of  CaCl2+Aq. 

Sp.  gr. 

1-normal 

j/r-    ;; 

Vs-        " 

1.0446 
1.0218 
1.0105 
1.0050 

(Calculated  by  Gerlach,  Z.  anal.  8,  283.) 


(Wagner,  Z.  phys.  Ch.  1890,  5.  36.) 


Sp.  gr.  at  16°/4°  of  CaCl2+Aq  containing 
12.1638%  CaCl2  =  1.10489.  (Schonrock,  Z. 
phys.  Ch,  1893,  11.  768.) 


CALCIUM  CHLORIDE 


147 


Sp.  gr.  of  CaCl2+Aq  at  17.925°C. 

B.-pt.  of  CaCl2 
100  pts.  H 
(Z.  anal.  2 
grand  (A. 

-f-Aq  containin 
2O     G  —  accord 

I  pts.  CaCl2  to 
ing  to  Gerlach 
cording  to  Le- 

% 

CaCh 

Sp.  gr. 

CaCU 

Sp.  gr. 

% 

CaCl» 

Sp.  gr. 

6.  440);  L  =  ac 
3h.  (2)  39.  43). 

0.0 
0.1 
0.2 
0.3 
0.4- 
0.6 
0.8 
1.0 
1.5 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 

0.99869 
0.99954 
1.00037 
1.00116 
1.00201 
1.00371 
1.00539 
1.00703 
1.01127 
1.01548 
1  .  02386 
1.03238 
1.04089 
1.04951 
.05822 
.06680 
1.07569 
.08467 
1.09373 
1  .  10288 

13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 

.11206 
.  12130 
.  13067 
.  14016 
.  14960 
.  15926 
.  16920 
.  17910 
1.18897 
1.19901 
1.20901 
1.21918 
1  .  22941 
1.23969 
1.25030 
1.26092 
1.27182 
1.28271 
1.29360 
1.30461 

33 
34 
35 
36 
37 
38 
39 
40 
41 
42 
43 
44 
45 
46 
47 
48 
49 
50 
51 

1.31562 
.32689 
.33821 
.34956 
.36100 
.37242 
1.38400 
1.39489 
1.40641 
1.41770 
.42882 
.44007 
.45124 
.  46238 
.47329 
.48450 
.49573 
.50676 
.51778 

B.-pt 

G 

L 

B.-pt. 

G 

L 

101° 
102 
103 
104 
105 
106 
107 
108 
109 
110 
111 
112 
113 
114 
115 
116 
117 
118 
119 
120 
121 
122 
123 
124 
125 
126 
128 
130 
130.4 
132 

6.0 
11.5 
16.5 
21.0 
25.0 
29.0 
32.5 
35.5 
38.5 
41.5 

55^0 
69.0 

ioi 

102.67 

10 
16.5 
21.6 
25.8 
29.4 
32.6 
35.6 
38.5 
41.3 
44.0 
46.8 
49.7 
52.6 
55.6 
58.6 
61.6 
64.6 
67.6 
70.6 
73.6 
76.7 
79.8 
82.9 
86.0 
89.1 
92.2 
98.4 
104.6 

110.9 

134° 
135 
136 
138 
140 
142 
144 
145 
146 
148 
150 
152 
154 
155 
156 
158 
160 
162 
164 
165 
166 
168 
170 
172 
174 
175 
176 
178 
179.5 

119 
137^5 
157 
178 
200" 
222 
245 
268  ' 

292 
305 

117.2 

123.5 
129.9 
136.3 
142.8 
149.4 

156^2 
163.2 
170.5 
178.1 
186.0 

194^3 
203.0 
212.1 
221.6 
231.5 

241.9 
252.8 
264.2 
276.1 
285.5 

301.4 
314.8 
325.0 

(Pickering,  B.  1894,  27.  1385.) 
Sp.  gr.  of  CaCl2+Aq  at  t°. 

t 

Concentration  of  CaCh  +Aq 

Sp.  gr. 

20 
20 

1  pt.  CaCl2  in  7.1045  pts.  H2O 
1    "        "     "  164.25     "      " 

1.1062 
1.0032 

(Hittorf,  Z.  phys.  Ch.  1902,  39.  628.) 
Sp.  gr.  of  CaCl2+Aq  at  20°. 

B.-pt.  of  CaCl2+Aq. 

%  CaCl2           B.-pt. 

%  CaCU            B.-pt. 

g.  mols.  CaCh  per  1.                            Sp.  gr. 

5.6             101° 
10.3             102 
14.5             103 

17.5             104° 
20.0             105 

0.010                                .000982 
0.025                                .002539 
0.050                                .004874 
0.075                                .006814 
0.10                                  .008971 
0.25                                  .02267 
0.50                                 .04451 
0.75                                  .06641 
1.00                               1.08744 

(Skinner,  Chem.  Soc.  61.  340.) 

Less  sol.  in  HCl+Aq  than  in  H2O.    HCl-h 
Aq  sat.  at  12°  dissolves  27%  CaCl2,  which 
crystallizes  out  with  2H2O.    (Ditte,  C.  R.  92. 

242.) 

Solubility  of  CaCl2  in  HCl+Aq  at  0°. 

(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38.  606.) 

Sat.  CaCl2+Aq  forms  a  crust  at  150°,  and 
contains   178  pts.   CaCl2  to   100  pts.   H2O. 
(Gerlach.) 
Sat.  CaCl2+Aq  boils  at  180°.    (Riidorff.) 

Sp.  gr.  of 
solutions 

g.  per  100  cc.  solution 

CaCIj 

HCl 

1.367 
1.344 
1.326 
1.310 
1.283 
1.250 
1.238 

51.45 
46.45 
42.80 
36.77 
29.84 
20.12 
11.29 

0.0 
3.32 
5.83 
10.66 
15.84 
23.05 
34.62 

(Engel,  C.  R.  1887,  104,  434.) 

148 


CALCIUM  CHLORIDE 


CaCl2+CaO2H2.    Solubility  of  CaCl2  + 
CaO2H2  in  H2O  at  25°. 

Solubility  of  CaCl2,  4CH3OH  in  CH3OH. 

t 

%  by  weight  of  CaCh,  4CH3OH 

CaCh 

CaO°2H2 

Solid  phase 

0 
10 
20 
30 
40 
50 
55 
56 

33.3 
37.6 
42.2 
47.0 
52.0 
57.3 
60.0 
61.3 

5.02 
10.00 
12.94 
15.14 
17.20 
18.15 
18.01 
21.02 
23.80 
24.33 
28.37 
29.54 
32.67 
33.21 
33.72 

34.36 
38.61 
41.32 
44.30 
44.60 
44.77 

0.101 
0.115 
0.128 
0.140 
0.145 
0.148 
0.152 
0/147 
0.146 
0.147 
0.170 
0.180 
0.225 
0.245 
0.254 

0.173 
0.060 
0.048 
0.030 
0.029 

Ca02H2 

CaChHz-fCaCh,  4CaO.14H2O 
CaCh,  4CaO.14H2O 

Ca02H2(?) 
CaCh,  4CaO.14H2O 
CaCh,  4Ca0.14H20+CaCh, 
Ca0.2H20 
CaCh,  CaO.2H20 

CaCh,  6H20+CaCl2,  CaO.2H2O 
CaCl2.6H20 

Solubility  of  CaCl2,  3CH3OH  in  CH3OH. 

t° 

%  by  weight  of  CaClz,  3CH3OH 

55 
75 
95 
115 
135 
155 
165 
170 
174 
177  (mpt.) 

60.5 

63.1 
66.3 
70.3 
75.2 

81.8 
86.2               U 
89.5 
93.5 
100 

(Menschutkin,  Z.  anorg.  1907,  62.  21.) 

(Schreinemakers  and  Figee,  Chem.  Weekbl. 
1911,  8.  685.) 

See  also  under  Calcium  hydroxide 


CaCl2 +KC1.  100  pts.  H2O  dissolve  56  pts. 
CaCl2  at  7°;  100  pts.  H2O  dissolve  31  pts. 
KC1  at  7°;  100  pts.  H2O  dissolve  63.5  pts. 
CaCl2+4.9  pts.  KC1  at  7°.  (Mulder,  J.  B. 
1866.  67.) 

CaCl2+NaCl.     100  pts.  H2O  dissolve  53 

S,s.  CaCl2  at  4°,  and  56  pts.  at  7°;  100  pts. 
2O  dissolve  35.7  pts.  NaCl  at  4°,  and  35.7 
pts.  at  7°;  IOC  pts.  H2O  dissolve  57.6  pts. 
CaCl2+2.4  pts.  NaCl  at  4°;  100  pts.  H2O  dis- 
solve 59.5  pts.  CaCl2+4.6  pts.  NaCl  at  7°. 
(Mulder,  I.  c.) 

100  g.  H2O  dissolve  72.6  g.  CaCl2  +  16.0  g. 
NaCl  at  15°.  (Riidorff.) 

Sol.  in  sat.  KNO3+Aq.    (Fourcroy.) 

Insol.  in  liquid  CO2.  (Biichner,  Z.  phys. 
Ch.  1906,  54.  674.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Sol.  in  1  pt.  strong  boiling  alcohol.  (Wen- 
zel.) 

Sol.  in  8  pts.  alcohol  at  15°,  and  in  1  pt. 
spirits  of  wine.  (Bergman.) 

Sol.  in  0.7  pt.  boiling  absolute  alcohol. 
(Otto.) 

Sol.  in  1.43  pts.  boiling  absolute  alcohol  at 
78.3°.  (Graham.) 

Solubility  of  CaCl2  in  methyl  alcohol. 

CaCl2  forms  with  methyl  alcohol  two  com- 
plexes: CaCl2.4CH3OH  and  CaCl2.3CH3OH. 


Solubility  of  CaCl2  in  ethyl  alcohol. 

CaCl2  forms  with  ethvl  alcohol  a  complex, 
CaCl2.3C2H5OH. 

Solubility    of    CaCl2.3C2H5OH    in    C2H5OH 
att°. 


t° 

%  by  weight  of 
CaCh.3C2H5OH 

t° 

%  by  weight  of 
CaCl'2.3C2HbOH 

0 

34.8 

80 

86.8 

20 

46.0 

85 

89.2 

40 

58.7 

90 

91.9 

60 

73.0 

95 

96.2 

70 

80.8 

97  mpt. 

100 

(Menschutkin,  Z.  anorg.  1907,  52.  23.) 

Sp.  gr.  at  1674°  of  CaCl2+alcohol  con- 
taining 5.668%  CaCl2  =  0.83636.  (Schonrock, 
Z.  phys.  Ch.  1893,  11.  768.) 

B.-pt.  of  an  alcoholic  solution  of  CaCl2. 


%  CaCh 

B.-pt. 

2.4 
5.39 
8.01 
9.93 
15.94 

78.43°+  0.70° 
78.43  +  2.15 
78.32  +  4.18 
78.43  +  5.55 
78.43  +11.75 

(Skinner,  Chem.  Soc.  61.  340.) 

SI.  sol.  in  propyl  alcohol.    (Berthelot.) 
100   g.    propyl    alcohol    dissolve    10.75    g. 

CaCl2.    (Schlamp,  Z.  phys.  Ch.  1894,  14,  276.) 
SI.  sol.  in  amyl  alcohol.    (Bouis.) 
Pptd.    from    alcoholic    solution    by    ether. 

(Dobbereiner.) 


CALCIUM  CHLORIDE 


149 


Sol.  in  wood-spirit;  sol.  in  lignone  (Liebig); 
insol.  in  lignone.  (Gmelin.) 

Insol.  in  acetone;  sol.  in  butyl  alcohol. 
(Wurtz.) 

Very  si.  sol.  in  acetone.  (Krug  and 
M'Elroy,  J.  Anal.  Ch.  6.  184.) 

Solubility  in  acetone +Aq  at  20°. 


Sol.  in  many  compound  ethers,  as  ethyl 
acetate  (Liebig),  ethyl  lactate  (Strecker). 

Sol.  in  considerable  quantity  in  amyl  sul- 
phocyanide.  (Medlock,  Chem.  Soc.  1.  374.) 

Sol.  in  valyl.    (Kolbe.) 

Very  sol.  in  cone.  HC2H3O2.    (Liebig.) 

Solubility  of  CaCl2  in  acetic  acid. 


CaCl2   will   salt   out   acetone  from   aqueous 
solution.    The  table  shows  the  composi- 

V^CtV^J.2      1W1111O        Wltll       CVVVVIW       dl/lvl       Ct       ljVlll£Jl.  \7JVp 

CaCl2,  4CH3COOH. 

tion  of  the  solutions  at  the  points  at 
which  inhomogeneous  solutions  of  CaCl2, 
acetone  and  H2O  just  become  homogen- 

Solubility of  CaCl2,  4CH3COOH  in 
CH3COOH  at  t°. 

eous  at  20°  .   1  00  g  .  of  the  solution  c  ontain  : 

t° 

%  by  wt.  CaCh,  4CH3COOH 

g.  CaCl2 

g.  H20 

K.   acetone 

11.1 

42.0 

QA 

47  fi 

13.03 

52.49 

34.48 

ou 

35 

TT  /    .  U 

50.0 

.    8.5 

45.37 

46.15 

40 

54.7 

6.38 

39.51 

54.11 

45 

63.0 

5.35 

35.95 

58.70 

50 

69.5 

4.11 

31.8 

64.09 

60 

79.5 

3.58 

29.88 

66.54 

65 

84.5 

3.31 

28.59 

68.10 

70 

91.2 

3.04 

27.03 

69.93 

*7f\      CT£* 

73 

100.0 

2.77 
13.90 

26.67 
53.47 

70.56 
32.63 

(Menschutkin 

,  Z.  anorg.  1907,  54.  95.) 

10  12 

48  86 

41  02 

-Ll_f  .    i  — 

8.47  • 

45  '.59 

45  '.94 

Insol.  in  benzonitrile.    (Naumann,  B.  1914, 

6.92 
6.31 

41.24 
39.15 

51.84 
54.54 

47.  1370.) 
Insol.   in   ethyl   acetate.      (Naumann,    B. 

5.28 
4.94 
4.37 
1.99 

36.09 
34.72 
33.8 
23.38 

58.63 
60.34 
61.83 
74.63 

1910,  43.  314.) 
SI.  sol.  in  anhydrous  pyridine. 
Sol.  in  97%,  95%  and  93%  pyridine  +Aq. 
(Kahlenberg,  J.  Am.  Chem.  Soc.   1908,  30. 

1.6 
1.35 

18.787 
12.443 
10  70 

21.4 
19.92 
55.301 
52.153 
49  6i 

77.00 
78.73 
25.913 
35.404 
39  69 

1107.) 
100  g.  sat.  solution  of  CaCl2  in  sat.  sugar  + 
Aq  at  31.25°  contain  42.84  g.  sugar+25.25  g. 
CaCl2,  or  100  g.  H2O  dissolve  135.1  g.  sugar 
+79.9  g.  CaCl2  at  31.25°.     (Kohler,  Z.  Ver. 

9^59 

8.82 
7.48 

7   07 

47  '.75 
46.04 
42.75 
41    ^4 

42.66 
45.14 
49.77 
51  39 

Zuckerind,  1907,  47.  447.) 
+H*O.  (Bakhuis  Roozeboom.)     See  above. 
4-2H2O.    (Bakhuis  Roozeboom.)   See  above. 
+4H2O.      Two    modifications.      (Bakfcuis 

§  .  \j  i 

6.72 
30.04 
18.23 
15.49 
13.18 
11.40 
28.09 

TCi  .  t^X 

40.48 
49.39 
55.01 
54.00 
52.52 
50.20 
51.71 

52^8 
20.57 
26.76 
30.51 
34.3 
38.40 
20.20 

Roozeboom.)    See  above, 
a   and   /3   modifications    (a  =  stable  form.) 
(Kuznetzov,  C.  A.  1911,  842.) 
+6H2O.    Very  deliquescent.    Sol.  in  H2O 
with  absorption  of  much  heat. 
250  pts.  CaCl2+6H2O  with  100  pts.  H2O 
at  10.8°  lower  the  temp.  23.2°.    (Riidorff,  B. 

26.81 
22.67 
18.189 

52.01 
55.66 
56.21 

21.18 
21.67 
25.60 

'  Melts  in  crystal  H2O  at  28°  (Tilden,  Chem. 
Soc.  45.  409);  at  30.2°  (Bakhuis  Roozeboom.) 

31.21 
2.23 
1.82 
0.68 

48.00 
24.93 
22.27 

15.87 

20.81 

72.84 
75.89 
83.44 

Sat.  solution  in  H2O  contains  at: 
—22°     —17°      —5°       —5°        +4° 
31.5       32.4       35.1       35.2       36.5%  salt, 

0.58 

14.93 

84.49 

8°          22° 

29°          35°          49° 

0.45 

13.55 

86.00 

37.9       42.1       46.1       49.0       55.1%  salt, 

0.48 

14.49 

85  .  13 

0.27. 

12.31 

87.42 

63°         80° 

104°        115° 

0.20 

9.95 

89.85 

55.9       57.5       58.5       58.6%  salt. 

0.15 

9.05 

90.81 

(fitard,  A 

ch.  1894,  (7)  2.  532.) 

(Frankforter,  J.  Am.  Chem.  Soc.   1914,  36. 
1125.) 

Sat.    solution 

of    CaCl2+6H2O    contains 

150 


CALCIUM  HYDROXYLAMINE  CHLORIDE 


44.77  g.  CaCl2  at  25°.    (Schreinemakers  and 
Figee,  Chem.  Weekbl.  1911,  8.  685.) 
See  also  above. 

Solubility  of  CaCl2+6H2O  in  ethyl  alcohol-f- 
Aq  under  addition  of  increasing  amounts 
of  CaCl2. 


Per  cent  of  alcohol 
by  volume 

G.  CaCh 
added 

Grams  CaCl2  in 
5  cc.  of  solution 

92.3 

1.430 

97.3 

.409 

99.3 

.429 

1 

1 

.529 

( 

2 

.561      * 

t 

3 

.590 

t 

4 

.641 

1 

5 

.709 

(Bodtker,  Z.  phys.  Ch.  1897,  22.  510.) 

Calcium  hydroxylamine  chloride,  CaCl2, 

3NH2OH,  HC1. 

(Antonow,  J.  Russ.  Phys.  Chem.  Soc.  1905, 
37.  479.) 

Calcium  iodine   bichloride,   2IC13,    CaCl2  + 

8H2O. 

Hydroscopic.     (Weinland,  Z.  anorg.  1902, 
30.  142.) 

Calcium  mercuric  chloride,  CaCl2,  5HgCl2  + 

8H,0. 

Decomp.  by  cold  H2O,  which  dissolves  out 
CaCl2,  but  all  dissolves  on  heating,    (v.  Bons- 


dorff,  1829.) 

CaCl2,      2HgCl2+6H2O. 


Deliquescent. 


Very  sol.  in  H2O.    (v.  Bonsdorff.) 

CaCl2,  6HgCl2+6H2O.  Very  deliquescent. 
Decomp.  by  H2O.  (Stromholm,  J.  pr.  1902, 
(2)  66.  521.) 

Calcium  lead  chloride,  basic. 
See  Calcium  lead  oxychloride. 

Calcium  magnesium  chloride,  CaCL,  2MgCl2 
+  12H20. 

Min.  Tachhydrite.    Deliquescent. 

100  pts.  H2O  dissolve  160.3  pts.  at  18.75°. 
By  dissolving  20  pts.  in  80  pts.  H2O  the  temp. 
is  raised  7.75°.  (Bischof.) 

Calcium    mercuric    chloride,    basic,    CaCl2 

2HgO+4H20. 
See  Calcium  mercuric  oxychloride. 

Calcium     thallic     chloride,     2TlCl3,CaCl2  + 
6H2O. 

Can  be  cryst.  from  H2O.  (Gewecke  A 
1909,  366.  222.) 

Calcium  tin  (stannic)  chloride. 
See  Chlorostannate,  calcium. 


Calcium  uranium  chloride,  CaCl2,UCl4. 

Decomp.  by  H2O.  (Aloy,  Bull.  Soc.  1899, 
(3)  21.  265.) 

Calcium  zinc  chloride. 

CaZnCl4+5>fH2O,  and  Ca2ZnCl6+6H2O. 
Very  hydroscopic.  (Ephraim,  Z.  anorg.  1910, 
67.  379.) 

Calcium  chloride  ammonia,  CaCl2,  8NH3. 
Sol.  in  H2O  with  decomp.     (Faraday.) 

Calcium  chloride  hydrazine,  CaCl2,  2N2H4(?). 
Ppt.    (Franzen,  Z.  anorg.  1908,.  60.  288.) 

Calcium  chloride  hydroxylamine,  CaCl2, 
NH2OH+5H2O. 

Not  hygroscopic.  (Antonow,  J.  Russ. 
Phys.  Chem.  Soc.  1905,  37.  479.) 

CaCl2,  2NH2OH. 

-f-H2O.  Aqueous  solution  sat.  at  20°  con- 
tains 56.6  pts.  salt. 

+2H2O.     (Antonow,  I.  c.) 

2CaCl2,  3NH2OH+6H2O.    (Antonow,  I.  c.) 

2CaCl2,  5NH2OH  +4H2O.    (Antonow,  1.  c.) 

Calcium  chloride  lead  oxide,  CaCl2,  3PbO  + 

3H2O. 
See  Calcium  lead  oxychloride. 

Calcium  chloroferrite,  CaO,  CaCl2,  Fe2O3. 
Insol.  in  H2O.    (le  Chatelier,  C.  R.  99.  276.) 

Calcium  chlorofluoride,  CaF2,  CaCl2. 

Decomp.  by  H2O,  by  very  dil.  HC1,  HNO3 
or  acetic  acid,  by  hot  dil.  or  cone.  H2SO4. 
Sol.  in  cone.  HC1  or  HNO3.  Insol.  in,  and  not 
decomp.  by  cold  or  boiling  alcohol.  (Defacqz, 
A.  ch.  1904,  (8)  1.  355.) 

Calcium   cyanamide,   basic,   CN2(CaOH)2-f 

6H2O. 

SI.  sol.  in  H2O.  (Meyer,  J.  pr.  1878,  (2)  18. 
425.) 

Calcium  cyanamide,  CaCN2. 

Decomp.  by  H2O.  (Meyer,  J.  pr.  1878,  (2) 
18.  425.) 

Calcium  swbfluoride,  CaF. 

Decomp.  by  H2O. 

Sol.  in  hot  dil.  HC1  and  somewhat  sol.  in 
dil.  acetic  acid. 

Somewhat  sol.  in  boiling  abs( 
(Wohler,  Z.  anorg.  1909,  61.  81.) 

Calcium  fluoride,  CaF2. 

Sol.  in  26,923  pts.  H2O  at  15.5°.  (Wilson, 
Ch.  Gaz.  1850.  366.) 

1  1.  H2O  dissolves  16  mg.  CaF2  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1904,  50.  356.) 

16.3  mg.  in  1  1.  of  sat.  solution  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1908,  64.  168.) 


CALCIUM  HYDROXIDE 


151 


When  pptd.  not  completely  insol.  in  H2O; 
scarcely  sol.  in  dil.,  more  sol.  in  cone.  HCl-f 
Aq;  decomp.  by  cone.  H2SO4;  not  decomp.  by 
dil.  alkaline  solutions.  (Fresenius.) 

Not  decomp.  by  cone.  H2SO4  below  40°,  but 
forms  a  transparent  syrup.  CaF2  is  pptd. 
from  this  solution  by  addition  of  H2O. 

Sol.  in  cone.  HC1,  and  HNO3+Aq  in  the 
same  way,  but  the  liquid  is  not  viscid.  Very 
si.  sol.  in  HF.  Boiling  HCl+Aq  dissolves 
slightly.  Decomp.  by  boiling  HNO3+Aq. 

Sol.  in  NH4  salts +Aq.    (Rose.) 

Partly  decomp.  by  boiling  K2CO3,  and 
Na2CO3+Aq.  (Dulong,  A.  ch.  82.  278.) 

Insol.  in  liquid  HF.  (Franklin,  Z.  anorg. 
1905,  46.  2.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Insol.  in  methyl  acetate.     (Naumann,  B. 

1909,  42.  3790.) 

Insol.   in   ethyl   acetate.      (Naumann,    B. 

1910,  43.  314.) 

Min.  Fluorite  (Fluorspar).  Calculated 
from  electrical  conductivity  of  CaF2+Aq, 
1 1.  H2O  dissolves  14  mg.  CaF2  at  18°.  (Kohl- 
rausch  and  Rose,  Z.  phys.  Ch.  12.  241.) 

Calcium  hydrogen  fluoride,  CaH2F4+6H2O. 

Decomp.  by  boiling  H2O.    Sol.  in  HF+Aq. 

(Fremy,  A.  ch.  (3)  47.  35.) 

Calcium  tantalum  fluoride. 
See  Fluotantalate,  calcium. 

Calcium  stannic  fluoride. 
See  Fluostannate,  calcium. 

Calcium  titanium  fluoride. 
See  Fluotitanate,  calcium.         4: 

Calcium  fluoiodide,  CaF2,CaI2. 

Very  deliquescent.  Decomp.  by  cold  H2O, 
more  rapidly  by  hot  H2O,  by  dil.  HC1,  HNO3, 
H2SO4  cone.  H2SO4,  and  by  alcohol  and  by 
ether  if  these  reagents  are  not  absolute.  (De- 
facqz,  A.  ch.  1904,  (8)  1.  358.)  % 

Calcium  hydride,  CaH. 

Decomp.  by  HCl+Aq.  (Winkler,  B.  24. 
1975.  (Moldenhauer,  Z.  anorg.  1913,  82. 136.) 

CaH2.  Readily  decomp.  by  H2O  and  dil. 
acids,  almost  insol.  in  cone,  acids.  Insol.  in 
benzene,  turpentine  and  alkyl  haloids.  (Mois- 
san,  C.  R.  1898,  127.  30-31.) 

Decomp.  H2O  and  ether;  sol.  in  dil.  H2SO 
and  HNO3:  almost  insol.  in  cone.  H2SO4  and 
HNO3.  (von  Lengyll,  C.  C.  1898,  II.  262.) 

Insol.  in  CC14,  CS2,  alcohols  and  ethers. 
No  known  solvent.  (Moissan,  C.  C.  1903,  I. 
863.) 

Calcium  hydrosulphide,  CaS2H2. 

Cry st.  with  6H2O.  Extremely  sol.  in  H2O 
and  alcohol.  l/i  of  its  weight  of  H2O  at  or- 


dinary temp,  more  than  suffices  to  hold  it  in 
solution.  (Divers  and  Shimidzu,  Chem.  Soc. 
46.  271.) 

Sp.  gr.  of  aqueous  solution  containing  32% 
anhydrous  CaS2H2  (64%  CaS2H2+6H2O)  = 
1.255:  37.5%  CaS2H2  (75.5%  CaS2H2  + 
6H2O)  =  1 .310.  (Divers  and  Shimidzu.) 

Calcium  hydroxide,  CaO2H2. 
See  also  Calcium  oxide. 
SI.  sol.  in  cold,  and  less  in  hot  H2O. 

1  pt.  CaO  dissolves  at  t°  in  pts.  H2O. 


t° 

Pts.  HzO 

Authority 

20 

450 

Davy. 

0 

656 

Phillips  (A.  Phil.  17..  107) 

700 

Bei 

uni 

an  (Essa 

VS.  ( 

itC.). 

13 

785 

Pavesi 

and  Rotondi  (B. 

7.  817) 

18 

780 

Bin 

eai 

(A.  ch. 

(3) 

51.  2< 

W), 

19.5 

806 

P.  and 

R.  (I.  c.). 

23 

814 

P. 

ind 

R.  (I.  c. 

18.75 

960 

Ab 

. 

54.4 

972 

Dalton  (Syst.  2.  231). 

15.6 

778 

Da 

!toi 

I   (I.   C.). 

15.6 

752 

Ph 

nip 

s  (I.  c..). 

15.6 
15.6 

731 

741 

Wittstein  (Repert.  Pharm.  1.  182). 
Tichborne  (Bull.  Soc.  (2)  17.  24). 

100 

1270 

Dalton  (I.  c.). 

100 

1280 

Ph 

Hip 

s  (I.  c.). 

100 

1330 

Wi 

ttst 

ein  (I.  c. 

100 

1340 

Tichborne  (I.  c.). 

100 

1500 

Bir 

irill 

1   (I.  C.). 

ICO 

1758 

Tichborne  (I.  c.). 

Solubility  in 
sat. 

H2O.     1000  pts.  CaO2H2+Aq 
at  t°  contain  pts.  CaO. 

t° 

Pts.  CaO 

T- 

From  Nitrate 

Marble 

Hydrate 

0 

1.362 

1.381 

] 

.430 

10 

1.311 

1.342 

] 

.384 

15 

1.277 

1.299 

1 

.344 

30 

1.142 

1.162 

] 

.195 

45 

0.996 

1.005 

; 

.033 

60 

0.884 

0.868 

0.885 

100 

0.562 

0.576 

0.584 

(Lamy,  C. 

R.  86. 

333 

•) 

Solubility  of  CaO2H2  in 

H2O  at  t°. 

Pts.  H20 

Pts.  CaO 

Pts 

H2O 

Pts.  CaO 

t° 

to  1  pt. 
CaO 

in  100 
pts.  H2O 

t° 

to  1  pt. 
CaO 

in  100 
pts.  H2O 

0 

759 

0.131 

60 

1136 

0.088 

10 

770 

0.129 

70 

1235 

0.080 

20 

791 

0.126 

80 

1362 

0.073 

30 

862 

0.116 

90 

1579 

0.063 

40 

932 

0.107 

100 

1650 

0.060 

50 

1019 

0.098 

(Maben,  Pharm.  J.  Trans.  (3)  14.  505.) 

1  pt.  CaO2H2  is  sol.  in  640  pts.  H2O  at  19°, 
and  3081  pts.  at  150°.  (Shenstone  and  Cun- 
dall,  Chem.  Soc.  63.  550.) 

1000  g.  H2O  dissolve  1.251  g.  CaO.  (Carles, 
Arch.  Pharm.  (3)  4.  558.) 


152 


CALCIUM  HYDROXIDE 


Solubility  of  CaO2H2  in  H2O.     100  pts.  H2O 
dissolve  pts.  CaO  at  t°. 

Sol.  in  H3BO3+Aq  at  30°.     (Sborgi,  Real. 
Ac.  Line.  1913,  (5)  22.  I,  715  and  798.) 
Sol.  in  NH4Cl-|-Aq.     Much  more  sol.  in 
NaCl+Aq  than  in  H2O.    (Rose.) 

Solubility  of  CaO2H2  in  NH4Cl+Aq  at  25°. 

t° 

Pts.  CaO 

t° 

Pts.  CaO 

20 
40 

60 

0.1374 
0.1162 
0.1026 

80 
100 

0.0845 
0.0664 

Concentration  of  NH4C1  +Aq 
in  millimols  per  liter 

Sorubility  of  CaO2H2  in 
millimols  per  liter 

(Zahorsky,  Z.  anorg.  3.  34.) 

1  pt.  CaO  is  sol.  in  pts.  H2O  at  t°. 
t°             15°   20°    25°    30°    35°    40°     45° 
pts.  H2O     776  813  848  885  924  962    1004 

0.00 
21.76 
43.52 
87.03 

20.22 
29.08 
39.23 
59.68 

t°     50°  55°  60°  65°  70°  75°  80° 
pts.  H2O  1044  1108  1158  1244  1330  1410  1482 

(Herzfeld,  C.  C.  1897,  I,  932.) 

100  g.  sat.  CaO2H2+Aq  contain  g.  CaO 
at  t°: 

t°  5        10          15          20         25 

g.  CaO  0.135     0.1342  0.132     0.1293  0.1254 

t°  30          35          40         50          60 

g.  CaO  0.1219  0.1161  0.1119  0.0981  0.0879 

t°  70          80         90         100 

g.  CaO  0.0781  0.074     0.0696  0.0597 
(Guthrie,  J.  Soc.  Chem.  Ind.  1901,  20.  223.) 

Solubility  in  H2O  at  high  temp. 

1  litre  of  the  solution  contains  at: 
120°          150°          190° 
0.305        0.169        0.084  g.  CaO. 

(Herold,  Z.  elektrochem.  1905,  11.  421.) 
Solubility  in  H2O  at  t°. 


t° 

1  g.  CaO  is  sol.  in  g.  HzO  at  t° 

2 

768.5 

10 

786.8 

15 

804.3 

20 

826.4 

25 

868.7 

30 

908.2 

40 

988.1 

50 

1083.0 

60 

1179.0 

70 

1274.8 

80 

1368.1 

(Moody,  Chem.  Soc.  1908,  93.  1772.) 

Sat.  CaO2H2+Aq  contains  at: 

95°  76° 

0.0580         0.0705%  by  wt.  CaO. 

(Tschugaeff,  Z.  anorg.  1914,  86.  159.) 

100  g.  sat.  solution  of  CaO2H2  in  H2O  at 
25°  contain  0.117  g.  CaO2H2.  (Cameron  and 
Potter,  J.  phys.  Ch.  1911,  16.  70.) 

Reaaily  sol.  in  most  acids. 


-  — 

i 

|| 

i 

'1 

c*~ 

o*— 

<O 

+c1 

t° 

o^ 

O^5 

S^ 

U£? 

Ofe\ 

GN§ 

u"5 

o2 

02 

og 

0£ 

51 

20 

0.1370 

0.1661 

0.1993 

0.1857* 

0.1661* 

0.1630* 

40 

0.1160 

0.1419 

0.1781 

0.2249 

0.3030* 

0.3684* 

60 

0.1020 

0.1313 

0.1706 

0.2204 

0.2989 

0.3664 

80 

0.0936 

0.1328 

0.1736 

0.2295 

0.3261 

0.4122 

100 

0.0906 

0.1389 

0.1842 

0.2325 

0.3710 

0.4922 

(Noyes  and  Chapin,  Z.  phys.  Ch.  1899,  28. 

520.) 

Solubility  of  CaO2H2  in  CaCl2  +Aq.  100  pts. 
CaCl2+Aq  of  given  strength  dissolve  pts. 
CaO  at  t°. 


*  In  these  cases,  ppts.  of  3CaO,  CaCl2+15H2O  were 
formed. 

(Zahorsky,  Z.  anorg.  3.  34.) 

See  also   CaCl2+CaO2H2    under   Calcium 
chloride. 

Solubility  in  Ca(NO3)2+Aq  at  25°. 


«  J* 

IB 

Sp.,  gr. 

QJ§* 

g,g 

Solid  phase 

25°/25° 

^J§ 

o§ 

_e 

&i  a 

1  .  0249 

0.096 

3.38 

) 

1.0484 

0.109 

8.52 

Ca(OH)2 

1.0940 

0.125 

13.42 

) 

1  .  1383 

0.181 

20.73 

Ca(OH)2  and  solid  solution 

CaO,  xN205,  yH2O 

1  .  1840 

0.187 

28.98 

1.2101 

0.198 

32.84 

1  .  2287 

0.212 

36.83 

1  .  2290 

0.213 

37.55 

1.2541 

0.224 

40.25 

Solid  solution 

1.2581 

0.230 

41.98 

CaO,  xN2O5,  yH2O 

1  .  2826 

0.260 

47.00 

1.2905 

0.263 

47.16 

1.3337 

0.332 

58.67 

1  .  3735 

0.429 

69.40 

1.4195 

0.545 

83.03 

Solid  solution  CaO,  xN2O5, 

yH2O  and  Ca(NO3)2, 

1.4840 
1.5330 

0.449 
0.371 

99.70 
115.50 

^    Ca(NO3)2,  3MH2O 

1  .  5809 

0.303 

135.30 

Ca(NO3)2,  33^H2O  and 
Ca(N03)2,  4H20. 

1  .  5842 

0.000 

139.30 

Ca(N03)2,  4H20 

(Cameron   and   Robinson,    J.   phys.    Chem. 

1907,  11,  275.) 

CALCIUM  HYDROXIDE 


153 


Solubility  of  CaO2H2  in  Ca(NO3)2+Aq. 
Temp.  =25°. 


G.  per  100  «.  sat. 
solution 

Solid  phase 

CaO 

Ca(NQs)j 

0.1150 

0 

CaO2H2 

0.0978 

4.84 

0.1074 

9.36 

" 

0.1193 

13.77 

" 

0.1444 

22.46 

» 

0.1650 

27.83 

" 

0.1931 

32.94 

» 

0.2579 

40.66 

" 

0.3060 

44.44 

" 

0.2802 

45.28 

Ca2N2O7.3H2O 

0.2314 

47.79 

0.1894 

51.07 

if 

0.1659 

53.20 

" 

0.1486 

55.25 

« 

0.0836  !     57.72 

Ca(NO3)2.4H20 

0                 57.98 

" 

Temp.  =  100°. 


0.0561 

0 

CaO2H2 

0.0550 

2.42 

" 

0.0624 

4.91 

•  « 

0.1110 

15.39 

• 

0.1200 

16.10 

" 

0.155 

21.86 

i 

0.269 

33.03 

. 

0.480 

42.26 

• 

0.973 

50.94 

« 

1.261 

53.75 

• 

1.477 

55.40 

• 

1.476 

55.43 

• 

1.491 

55.65 

• 

1.635 

56.89 

CaO2H+Ca2N2O7.2H20 

1.686 

57.03 

Ca2N207.2H2O 

1.596 

57.91 

«< 

1.576 

58.67 

" 

1.348 

60.44 

«< 

1.167 

62.82 

•  • 

1.077 

66.44 

» 

1.141 

69.12 

» 

1.252 

70.60 

Ca2N2O7.2H2O+Ca2N207.^H2O 

1.203 

70.40 

CatNjOr.HHsO 

1.103 

71.44 

" 

0.937 

73.85    . 

" 

0.849 

75.74 

«« 

0.815 

76.94 

» 

0.804 

77.62 

Ca(NO3)2 

0.412 

77.74 

» 

0 

78.43 

«« 

(Bassett  and  Taylor,  Chem.  Soc.  1914,  106. 
1926.) 


Solubility  of  CaO  in  KC1  and  NaCl+Aq. 
Curves  are  given  which  show  that  the  solu- 
bility of  lime  in  solutions  of  either  NaCl  or 


KC1  is  a  maximum  for  all 

temps,  when  the 

solution  contains  about  60 

g.  of  salt  per  1. 

It  is  a  minimum  at  any  fixed  temp,  when  the 

solution   is   sat.,   the  solubility   then   beine 

much  less  than  in  pure'H2O 

of  the  same  temp. 

A  solution  of  NaCl  dissolves  more  lime  at  all 

temps,  and  concentrations  than  a  correspond- 
ing solution  of  KC1.  In  all  cases  the  maximum 

solubility  of  lime 

occurs  when  the 

temp,  is 

lowest.    With  solutions  of  all  concentrations 

the  solubility  decreases  regularly  as  the  temp. 

increases.    (Cabot, 

J.  Soc.  Chem.  Ind.  1897, 

16.  417-419.) 

Solubility  in  KCl+Aq  increases 

with  in- 

creased  quantities 

of  KC1 

and  then  dimin- 

ishes,  becoming  le 

ss  than 

the  solubility  in 

H2O  alone.     (Kernot,  Gazz 

.  ch.  it.  1908,  38. 

(1)  532.) 

KOH  or  NaOH+Aq  containing  1  pt.  KOH 
or  NaOH  in  100  pts.  H2O  do  not  dissolve 

more  than  Vsoooo  pt.  CaO2H2,  but  it  is  sol.  in 

NH4OH+Aq.    (Pelouze,  A. 

ch.  (3)33.11.) 

Solubility  in  NaOH+Aq  at  t°. 

G.  NaOH 

Solubility  of  CaO  in  g.  per  liter  at 

perl 

20° 

50° 

70° 

100° 

0 

1.17 

0.88 

0.75 

0.54 

0.400 

0.94 

0.65 

0.53 

0.35 

1.600 

0.57 

0.35 

0.225 

0.14 

2.666 

0.39 

0.20 

0.11 

0.05 

5.  .000 

0.18 

0.06 

0.04 

0.01 

8.000 

0.11 

0.02 

0.01 

traces 

20.000 

0.02 

traces 

0 

0 

(d'Anselme,  Bull 

.  Soc.  1903,  (3)  29. 

936.) 

Solubility  of  CaO  in  NaCl+NaOH+Aq. 

GTVaPl 

G.  CaO 

per  1.  of  solution  containing 

.     IN  £101 

perl. 

.   _TT            0.89  g.                4.09  g. 
No  NaOH      NaOH  per  1.    NaOH  per  1. 

0 

1.3 

0.8 

0.22 

5 

1.4 

0.9 

10 

1.6 

1.0 

25 

1.7 

1. 

L 

50 

1.8 

1.25 

75 

1.9 

1.4               0.55 

100 

1.85 

1.4 

150 

1.65 

1.25             0.44 

175 

1.6 

1.2 

182 

1.6 

1.2 

225 

1.4 

1.0 

250 

1.3 

0.9                

300 

1.1 

0.7               0.22 

(Maigret,  Bull. 

Soc.  1905,  (3)  33.  631.) 

154 


CALCIUM  HYDROXIDE 


Solubility  of  CaO2H2  in  CaSO4+Aq  at  25C 


G.  per  100  cc.  sat. 
solution 

Solid  phase 

CaSOi 

CaO 

0 

0.1166 

Ca02H2 

0.0391 

0.1141 

" 

0.0666 

0.1150 

" 

0.0955 

0.1215 

'• 

0.1214 

0.1242 

" 

0.1588 

0.1222 

CaO2H2  fCaSO4.2H2O 

0.1634 

0.0939 

CaS04.2H20 

0.1722 

0.0611 

0.1853 

0.0349 

" 

0.1918 

0.0176 

" 

0.2030 

0.0062 

" 

0.2126 

0 

" 

(Cameron  and  Bell,  J.  Am.  Chem.  Soc.  1906, 
28.  1220.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Alcohol  dissolves  traces. 

Methyl  alcohol  forms  colloidal  solution 
containing  1.125  g.  per  1.  (Neuberg  and 
Rewald,  Biochem.  Z.  1908,  9.  545.) 

Insol.  in  ether. 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329 .) 

Insol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1904,  37.  3601.) 

Much  more  sol.  in  glycerine,  or  sugar +Aq 
than  in  H2O. 


Solubility  of  CaO  in  glycerine. 


Wt.  of 
glycerine  in 

Wt.  CaO 

contained  in 
100  ccm.  of 

Relation  of  CaO  to 
glycerine 

solution 

liquid  sat. 
with  CaO 

CaO 

Glycerine 

10.00 

0.370 

3.6 

96.4 

5.00 

0.240 

4.6 

95.4 

2.86 

0.196 

6.4 

93.6 

2.50 

0.192 

7.1 

92.9 

2.00 

0.186 

8.5 

91.5 

1.00 

0.165 

14.2 

85.8 

(Berthelot,  A.  ch.  (3)  46.  176.) 


1000  g.  H2O  dissolve  1.251  g.  CaO;  1000  g. 
H2O-t-50  g.  glycerine  dissolve  1.865  g.  CaO; 
1000  g.  H2O  +  100  g.  glycerine  dissolve  2.583 
g.  CaO;  1000  g.  H2O+200  g.  glycerine  dis- 
solve 4.040  g.  CaO;  1000  g.  H2O+400  g. 
glycerine  dissolve  6.569  g.  CaO.  (Carles, 
Arch.  Pharm.  (3)  4.  558.) 

Insol.  in  pure  glycerine. 


Solubility  of  CaO2H2  in  glycerine +Aq  at  25°. 

G  =  g.  glycerine  in  100  g.  glycerine +Aq. 

^Ca(OH2)=millimols  sol.  in  100  cc.  glyc- 
erine+Aq. 


G 

HCa02H2 

Sp.   gr. 

0 
7.15 
20.44 
31.55 
40.95 
48.7 
69.2 

4.3 
8.13 
14.9 
22.5 
40.1 
44.0 
95.8 

1.0003 
1.0244 
1.0537 
1.0842 
1.1137 
1  .  1356 
1  .  2027 

(Herz  and  Knoch,  Z.  anorg.  1905,  46.  193.) 


Solubility  in  glycerine +Aq  at  25°. 


Solution  contains 

Sp.  gr. 

%   Ca(OH)2 

%  glycerine 

%H20 

0.117 
0.178 
0.413 
0.48 
0.88 
1.34 

0 
3.50 
15.59 
17.84 
34.32 
55.04 

96^32 
80.28 
81.68 
64.80 
43.62 

1^008 

1.042 
1.088 
1.149 

Solid  phase  in  this  system  is  CaO2H2. 
(Cameron  and  Patten,  J.  phys.  Chem.  1911, 
15.  71.) 


100  pts.  sugar  dissolved  in  H2O  dissolve  55.6  pts. 
CaO  (Osann);  50  pts.  CaO  (Ure) ;  49.6  pts.  CaO 
(Daniell);  29-30.6  pts.  CaO  (Hunton) ;  23  pts.  CaO. 
(Soubeiran.) 

Sugar  solution  at  100°  takes  up  M  rnol.  CaO  for  each 
mol.  sugar;  at  0°,  if  it  contains  not  less  than  25%  of 
sugar,  it  takes  up  2  mols.  CaO  to  1  mol.  sugar.  (Du- 
brunfaut.) 

Amount  dissolved  is  proportional  to  the  density  and 
temperature  of  the  solutions. 


Solubility  of  CaO  in  sugar  +Aq. 


Pts.  sugar 
dissolved  in 
100  pts.  H2O 

Relation  of  CaO  to  sugar 

CaO 

Sugar 

40 

21.0 

79.8 

37.5 

20.8 

79.2 

35.0 

20.5 

79.5 

32.5 

20.3 

79.7 

30.0 

20.1 

79.9 

27.5 

19.9 

80.1 

25.0 

19.8 

80.2 

22.5 

19.3 

80.7 

20.0 

18.8 

81.2 

17.5 

18.7 

81.3 

15.0 

18.5 

81.5 

12.5 

18.3 

81.7 

10.0 

18.1 

81.9 

7.6 

16.9 

83.1 

5.0 

15.3 

84.7 

2.5 

13.8 

86.2 

(Peligot,  C.  R.  32.  335.) 


100  g.  solution  of  sugar  sat.  with  CaO  between  10° 
and  54.4°  contain  22.5  to  23.5%  CaO.     (Hunton,  1837.) 


CALCIUM  HYDROXYHYDROSULPHIDE 


155 


Solubility  of  CaO  in  dil.  sugar  solutions. 


Wt.  of  sugar 
in  100  ccm. 

Wt.  of  CaO 
contained  in 
100  ccm.  of 

Relation  of  CaO 
to  sugar 

of  solution 

liquid  sat. 
with  CaO 

CaO 

Sugar 

4.850 

1.031 

17.5 

82.5 

2.401 

0.484 

16.8 

83.2 

2.000 

0.433 

17.8 

82.2 

1.660 

0.364 

18.0 

82.0 

1.386 

0.326 

19.0 

81.0 

1.200 

0.316 

20.8 

79.2 

1.058 

0.281 

21.0 

79.0 

0.960 

0.264 

21.6 

78  4 

0.400 

0.194 

32.7 

67.3 

0.191 

0.172 

47.4 

52.6 

0.096 

0.154 

61.6 

78.4 

0.000 

0.148 

(Berthelot,  A.  ch.  (3)  46.  176.) 


Solubility  in  sugar +Aq  at  t°. 


G.  sugar  in  100  ccm. 

G.  CaO  dissolved 

t° 

of  solution 

per  100  g.  sugar 

16-17° 

0.7814 

37.9 

0.9120 

32.3 

1.4000 

30.5 

1.6930 

28.9 

4.754 

27.7 

5.730 

27.1 

10.159 

27.5 

11.200 

27.2 

12.500 

27.3 

13.930 

27.9 

14.487 

27  5 

16.410 

28.0 

15C 

0.625 

71.6 

0.964 

53.4 

2.084 

36.0 

3.028 

32.3 

3.451 

31.7 

4.168 

30.2 

4.880 

28.7 

5.73 

28.3 

6.12 

27.4 

6.25 

27.7 

6.51 

27.5 

7.55 

27.9 

8.20 

27.3 

(Weisberg,  Bull.  Soc.  1899,  (3)  21.  775.) 


Solubility  in  sugar  +Aq  at  25°. 

Solution  contains 

Sp.  gr. 

%  Ca(OH)2 

%  sugar 

%  H20 

0.117 
0.188 
0.730 
1.355 
2.31 
3.21 
4.57 
5.38 
6.07 

0 
0.62 
4.82 
7.50 
9.87 
11.90 
15.10 
17.42 
19.86 

99^19 
94.50 
91.12 

87.85 
84.89 
80.33 
76.93 
73.07 

0.983 
.000 
.021 
.037 
.051 
.067 
1.092 
1.109 
1.123 

The  solid  phase  in  this  system  consists  of  a 
series  of  solid  solutions  with  Ca(OH)2  a  limit- 
ing case. 
(Cameron  and  Patten,  J.  phys.  Chem.  1911, 
15.  70.) 

Solubility  of  CaO  in  sugar  +Aq  at  80°. 

%  sugar 

%  CaO 

70  Sugar 

%CaO 

4.90 
9.90 
14.75 

0.117 
0.189 
0.230 

19.50 
24.60 
29.70 

0.358 
0.458 
1.017 

Solid  phase,  ,CaO2H2. 
(von  Ginneken,  Proc.  Kon.  Akad.  v.  Wet- 
ensch,  Amsterdam,  1911,  14.  457.) 

Solubility  of  CaO  in  mannite  +Aq. 

Wt.  of 
mannite  in 
100  ccm.  of 
solution 

Wt.  of  CaO 
contained  in 
100  ccm.  of 
liquid   sat. 
with  CaO 

Relation  of  CaO  to 
mannite 

CaO 

Mannite 

9.60 
4.80 
2.40 
.92 
.60 
.37 
.20 
.07 
0.96 
0.192 
0.096 
0.000 

0.753 
0.372 
0.255 
0.225 
0.207 
0.194 
0.193 
0.190 
0.186 
0.155 
0.154 
0.148 

7.3 

7.2 

9.6 
10.5 
11.4 
12.5 
13.9 
15.1 
16.2 
44.6 
61.6 

92.7 

92.8 
90.4 
89.5 
88.6 
87.5 
86.1 
84.9 
86.8 
55.4 
38.4 

(Berthelot,  A.  ch.  (3)  46.  176.) 
Solutions  of  CaO  in  sugar,  mannite,  or  gly- 

UCllllt/         Clli^Jl*-*.         C*A1         C*^-'V**AV*M;**  v         ffv»         v  -^"O 

heated,    but    this    redissolves    on    cooling. 
(Berthelot.) 

Sol.  in  sorbite+Aq  (Pelouze);  si.  sol. 
in  quercite+Aq.  Sol.  in  monobasic  Ca  sac- 
charate+Aq.  (Peligot.)  Much  more  sol.  in 
gelatine +Aq  than  in  pure  H2O. 

Calcium  hydroxyhydrosulphide,  Ca(OH)SH  + 

3H2O. 

Easily  sol.  in  H2O  with  almost  immediate 
decomposition.  Insol.  in  alcohol,  but  slowly 


156 


CALCIUM  IODIDE 


decomp.    thereby.      (Divers    and    Shimidzu, 
Chem.  Soc.  46.  270.) 

Calcium  subiodide,  Cal. 

Decomp.  by  moisture.  (Wohler,  Z.  anorg. 
1909,  61.  76.) 

Calcium  iodide,  CaI2. 

Deliquescent.    100  pts.  H2O  dissolve — 
at  0°         20°       40°       43°       92° 

192       204      228      286      435  pts.  CaI2. 
(Kremers,  Pogg.  103.  65.) 

Sp.  gr.  of  Cala+Aq  at  19.5°  containing: 
5  10        15         20        25       30%  CaI2, 

1.044     1.09     1.14     1.198     1.26    1.321 

35         40       45        50        55       60%  CaI2. 
1.398     1.477  1.567  1.665     1.78    1.91 
(Kremers,   calculated  by  Gerlach,   Z.   anal. 
8.  285.) 

Sol.  in  absolute  alcohol.  (Gay-Lussac,  A. 
ch.  91.  57.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328;  Eidmann,  C.  C.  1899,  II.  1014.) 

Sol.  in  ethyl  acetate.  (Naumann,  B.  1910, 
43.  314.) 

+4H2O.     (Kuznetzov,  C.  A.  1911.  842.) 

-j-6H2O.    Sat.  aq.  solution  contains  at: 
—22°      +7°         10°          19° 
61.6        65.0        65.1        66.3%  salt. 

51°          64°         130°        248° 
69.4        75.9        81.3        87.1%  salt. 
(Etard,  A.  ch.  1894,  (7)  2.  543.) 

+7H2O.     (Kuznetzov.) 

Calcium  pmodide,  CaI3+15H2O. 
(Mosnier,  A.  ch.  1897.  (7)  12.  401.) 
CaI4.    (Herz  and  Bulla,  Z.  anorg.  1911,  71. 

255.) 

Calcium  mercuric  iodide,  CaI2,HgI2+8H2O. 

Very  deliquescent.  Sol.  in  H2O,  alcohols, 
allyl  iodide,  aldehyde,  acetic  acid,  ethyl  oxal- 
ate  and  aniline.  SI.  sol.  in  nitrobenzene. 
Completely  insol.  in  CHC13,  CC14,  ethyl 
iodide,  ethylene  bromide,  C6H6,  monochlor- 
benzene  and  toluene.  (Duboin.  C.  R.  1906, 
142.  573.) 

3CaI2,  4HgI2+24H2O.  Sol.  in  H20  with 
pptn.  of  red  HgI2. 

Very  sol.  in  alcohols,  glycerine,  ethyl  ace- 
tate, methyl  and  isobutyl  propionate,  allyl 
iodide,  aldehyde,  acetone,  aniline  and  ethyl 
oxalate.  Insol.  or  si.  sol.  in  nitrobenzene. 
Insol.  in  CHC13,  C6H6,  ethyl  iodide,  mono- 
chlorbenzene,  etc.  (Duboin,  C.  R.  1906,  142. 
397.) 

CaI2,  2HgI2. 

Decomp.  by  H2O.    (Boullay.) 

CaI2,   5HgI2+8H2O.     Decomp.   by  H2O, 


alcohols,  glycerine,  aldehyde,  and  acetic  acid; 
slowly  by  nitrobenzene  and  ethyl  oxalate. 
Insol.  in^monochlorbenzene,  toluene,  CHC13 
and  ethylene  bromide.  (Duboin,  /.  c.) 

Calcium  silver  iodide,  CdI2,  2AgI+6H2O. 

Immediately  decomp.  by  H2O.  (Simpson, 
Roy.  Soc.  Proc.  27.  120.) 

Calcium  zinc  iodide,  CaI2,  ZnI2+8H2O. 

Very  hydroscopic.  (Ephraim,  Z.  anorg. 
1910,  67.  384.) 

Calcium  iodide  ammonia,  CaI2,  6NH3. 
(Isambert,  C.  R.  66.  1259.) 

Calcium  nitride,  Ca3N2. 

Sol.  in  dil.  acids;  insol.  in  cone,  (water  free) 
acids.  (Moissan,  C.  R.  1898,  127.  499.) 

Calcium  oxide,  CaO. 

Decomp.  by  H2O,  with  evolution  of  much 
heat,  to  form  CaO2H2,  which  see  for  solubility 
in  H2C,  etc. 

Calcium  peroxide,  CaO2. 

Very  si.  scl.  in  H2O;  easily  sol.  in  acids, 
and  NH4  salts +Aq.  Insol.  in  NH4OH+Aq. 
(Conroy,  Chem.  Soc.  (2)  11,  808.) 

-f2H2O.  True  composition  is  CaO2H2  + 
H2O2.  (de  Forcrand,  C.  R.  1900,  130.  1390.) 

+8H2O.  Efflorescent.  Difficultly  sol.  in 
H2O  with  gradual  decomp.  Insol.  in  alcohol 
or  ether.  (Gay-Lussac  and  Thenard,  A.  ch. 
(2)  8.  313.) 

Calcium  oxybromide,  3CaO,  CaBr2  +  16H2O. 
Decomp.  by  H2O  and  alcohol.    Very  easily 
sol.  in  hydracids  and  dil.  HNO3.     (Tassily, 
C.  R.  1894,  119.  372.) 

Calcium  oxychloride,  Ca4O3Cl2  +  15H2O  = 
3CaO,  CaCl2  +  15H2O. 

Decomp.  by  H2O  or  alcohol.    (Rose.) 

Formula  is  Ca2HO2Cl+7H2O.  (Grimshaw, 
C.  N.  30.  280.) 

+  16H2O.  Decomp.  by  H2O  into  CaO2H2 
and  CaCl2  until  a  maximum  of  85  g.  CaCl2 
are  dissolved  per  litre.  (Ditte,  C.  R.  91.  576.) 

4CaO,  CaCl2+14H2O.  (Schreinemakers 
and  Figee,  Chem,  Weekbl.  1911,  8.  685.) 

CaO,CaCl2.     (Schreinemakers  and  Figee.) 

Calcium  lead  oxychloride,  CaCl2,  CaO,  2PbO 
+4H20. 

Sol.  in  H2O  with  decomp.  (Andre,  C.  R. 
104.  359.) 

CaCl2,  3PbO+3H2O.    (Andre.) 

Calcium  mercuric  oxychloride,  CaCl2,  2HgO 

+4H20. 

Decomp.  immediately  by  H2O.  (Klinger, 
B.  16.  997.) 


CALCIUM  SULPHIDE 


157 


Calcium  oxyiodide,  3CaO,  CaI2  +  16H2O. 

Decomp.  by  H2O,  alcohol,  and  acids.  Sol. 
in  hydracids  and  in  very  dil.  HNO3.  (Tassily 
C.  R.  1894,  119.  372.) 

Calcium   oxysulphide,    Ca4O3S4  +  12H2O  = 
3CaO,  CaS4  +  12H2O. 

Decomp.  by  H2O.  Not  acted  on  by  ab- 
solute alcohol.  (Schone,  Pogg.  117.  77.) 

According  to  Geuther  (A.  224.  178)  =CaS3 
2CaO  +  10,  or  11H2O.  Sol.  in  dil.  HCl+Aq 
with  separation  of  S. 

Ca5O4S4  +  18H2O=4CaO,  CaS4  +  18H2O. 
Decomp.  by  H2O,  but  not  acted  on  by  ab- 
solute alcohol.    (Schone,  Pogg.  117.  82.) 

According  to  Geuther  (A.  224.  178)  =CaS3, 
3CaO  +  14,  or  15H2O. 

Ca6O5S5+20H2O=5CaO,  CaS6+20H2O. 
(Rose,  Pogg.  66.  433.) 

Sol.  in  400  pts.  cold,  decomp.  by  boiling 
H2O  (Buchner);  si.  sol.  in  cold,  much  more  in 
hot  H2O,  but  it  is  not  deposited  on  cooling. 
Aqueous  solution  sat.  at  6°-7.2°  has  sp.  gr.  = 
1.0105  (Herschel);  sol.  in  alcohol  (Gay-Lus- 
sac);  insol.  in  alcohol  (Gmelin). 

Calcium  phosphide,  CaP. 

Deliquescent.  Decomp.  in  moist  air  or 
with  H2O.  Not  attacked  by  cone.  HNO3,  but 
decomp.  by  dil.  HNO3+Aq.  (Thenard,  A. 
ch.  (3)  14.  14.) 

Ca3P2.    Crystallized. 

Decomp.  by  H2O. 

Not  attacked  by  cone.  H2SO4.  Violently 
attacked  by  dil.  H2SO4. 

Not  attacked  by  abs.  alcohol,  ether,  ben- 
zene or  oil  of  turpentine.  (Moissan,  C.  R. 
1899,  128.  792.) 

Ca2P3.  Insol.  in  liquid  CO2.  (Buchner, 
Z.  phys.  Ch.  1906,  64.  674.) 

Calcium  selenide,  CaSe. 

SI.  sol.  in  H2O.  Very  easily  decomp. 
(Fabre,  C.  R.  102.  1469.) 

Calcium  silicide,  CaSi2. 

Slowly  decomp.  by  H2O;  sol.  in  cone.  H2SO4 
and  dil.  HNO3  with  evolution  of  H2.  With 
cone.  HC1  it  gives  H2,  Si  and  silicon  hydride; 
with  dil.  HC1,  H2  and  a  yellow  substance. 
Sol.  in  alkali -j-Aq  or  NH3+Aq  with  evolu- 
tion of  H2.  (Moissan,  C.  R.  1902,  134.  505.) 

Two  modifications: 

(a)  Only  si.  sol.  in  HNO3;  decomp.  H2O  to 
give  an  insol.  ppt.  on  addition  of  HC1. 

(b)  Easily  sol.  in  HNO3  and  acetic  acid; 
decomp.  HC1  to  give  a  ppt.  which  is  sol.  in 
KOH+Aq.     (de  Chalmot,  Am.  Ch.  J.  1896, 
18,  320.) 

Ca3Si2.  Slowly  decomp.  by  H2O,  rapidly 
by  dil.  acetic  acid  or  by  H2SO3+Aq  without 
evolution  of  spontaneously  inflammable  gas. 
(Honigschmid,  M.  1909,  30.  497.) 

Decomp.  by  dil.  min.  acids,  with  evolution 


of  spontaneously  inflammable  gas.  (Hack- 
spill,  Bull.  Soc.  1908,  (4)  3.  619.) 

CaeSiio.  Insol.  in  all  solvents.  Decomp. 
by  boiling  H2O,  by  cone.  HC1  and  by  acetic 
acid.  Sol.  in  dil.  alkali  and  alkali  carbonates 
+Aq.  Hardly  attacked  by  cone.  H2SO4  or 
HN03.  (Kolb,  Z.  anorg.  1909,  64.  349.) 

CanSiio.  Easily  decomp.  by  boiling  with 
H2O.  Decomp.  by  dil.  acetic  acid,  dil.  or 
cone.  HC1.  (Kolb,  Z.  anorg.  1909,  64.  349 
and  356.) 

Calcium  siliconitride,  CaSi2N3. 

(Kolb,  Z.  anorg.  1909,  64.  363.) 

Ca2Si3N4.  Slowly  decomp.  by  boiling  with 
H2O,  somewhat  more  rapidly  with  dil.  NaOH 
+Aq.  Slowly  decomp.  by  cone.  HC1.  (Kolb, 
I.e.) 

CanSii0N10.  Completely  decomp.  by  HC1. 
(Kolb,  I.e.) 

Calcium  sulphide,  CaS. 

500  pts.  H2O  dissolve  1  pt.  CaS  completely; 
less  H2O  dissolves  out  CaS2H2  and  leaves 
CaO2H2.  Very  much  H2O  decomposes  com- 
pletely into  CaO2H2  and  H2S.  (Bechamp,  A. 
ch.  (4)  16.  222.) 

Not  decomp.  by  H2O,  and  only  si.  sol. 
therein  at  ordinary  temp.  (Pelouze.) 

After  48  hours  contact  with  CaS,  1  1.  H2O 
contains  at: 

10°        18°'      40°       60°       90° 

0.15      0.23      0.30      0.48      0.33  g.  CaS. 

After  boiling  for  2  hours,  0.27  g.  CaS  is 
dissolved;  addition  of  NaCl  diminishes  solu- 
.bility,  but  Na2SO4  increases  it.  Lime-water 
Dissolves  at  14°  0.18  g.  CaS,  the  same  amount 
which  H2O  dissolves  at  60°.  Milk  of  lime 
dissolves  0.55  g.  at  60°.  H2O  containing  3  to 
79  g.  Na2O  per  litre  dissolves  only  traces  of 
CaS  at  10°,  but  at  40-^60°,  or  by  boiling,  a 
large  amount  of  Na2S  is  formed.  (Kolb,  A. 
ch.  (4)  7.  126.) 

Sol.  in  12,500  pts.  H2O  at  12.6°.  (Scheurer- 
Kestner,  Repert.  chim.  appl.  1862.  331.) 

Sat.  Na2CO3+Aq  has  scarcely  any  action 
on  CaS,  but  a  dilute  solution  has  more  action. 
(Kolb.) 

Sol.  in  H2O  and  sulphur,  forming  CaS4. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1904,  37.  3601.) 

Insol.  in  methylal.  (Eidmann,  C.  C.  1899, 
II.  1014.) 

Sol.  in  10  pts.  glycerine.  (Cap  and  Garot, 
J.  Pharm.  (3)  26.  81.) 

Sol.  in  sugar +Aq.  (Stolle,  C.  C.  1900,  I. 
1044.) 

Calcium  tefrasulphide,  CaS4. 
Known  only  in  solution. 


158 


CALCIUM  SULPHIDE 


Calcium  pe«tasulphide,  CaS5. 

Sol.  in  H2O  and  alcohol.    (Berzelius.) 
Exists  only  in  aqueous  solution.     (Schone, 

Pogg.  117.  73.) 

Calcium    hydroxyl    sulphide,    Ca(OH)SH  + 

3H2O. 

Easily  sol.  in  H2O  with  immediate  decomp. 
and  separation  of  Ca(OH)2.  Insol.  in  alcohol, 
but  slowly  decomp.  thereby.  (Divers  and 
Shimidzu,  Chem.  Soc.  45.  270.) 

Calcium  stannic  sulphide. 
See  Sulphostannate,  calcium. 

Calomel. 
See  Mercurous  chloride. 

Carbamic  acid. 

Ammonium  carbamate  acid  carbonate  (com- 
mercial carbonate  of  ammonia) . 
See  Carbonate  carbamate,  ammonium  hy- 
drogen. 

(salts  of  hartshorn).  2NH4HCO3, 

NH4CONH2. 

See  Carbonate  carbamate,  ammonium  hy- 
drogen. ' 

Carbazote  silicon,  C2SiN. 

Insol.  in  acids,  even  HF;  also  in  boiling 
KOH+Aq.  (Schiitzenberger  and  Colson, 
C.  R.  92.  1508.) 

Carbon,  C. 

Insol.  in  all  solvents. 

Diamond  is  unacted  upon  by  KClO3+fum. 
HNO3;  graphite  forms  graphitic  acid  by 
KClO3+fum.  HNO3;  amorphous  carbon  fs 
sol.  in  KClO3+fum.  HNO3.  (Berthelot,  A. 
ch.  (4)  19.  399.) 

Diamond  is  sol.  in  molten  iron  at  1160°. 
Amorphous  carbon  is  insol.  in  molten  iron  at 
1160°,  but  becomes  sol.  therein  by  heating  to 
1400°.  (Hempel,  B.  18.  998.) 

Insol.  in  liquid  CO2.  (Buchner.  Z.  phys. 
Ch.  1906,  54.  674.) 

Charcoal  is  insol.  in  liquid  NH3.  (Gore, 
Am.  Ch.  J.  1898,  20.  830.) 

The  quantity  of  carbon  dissolved  by  iron 
diminishes  by  increasing  phosphorus,  falling 
by  about  0.5%  for  each  additional  2.0%  of 
phosphorus.  (Fettweis,  Metallurgie,  1906, 
3.  60.) 

Solubility  in  iron  is  reduced  by  the  presence 
of  tin  and  of  sulphur.  (Wiist,  Metallurgie, 
1906,  3.  169.) 

The  solubility  of  C  in  iron  is  increased  by 
the  presence  of  chromium;  9.2%  C  dissolved 
when  62%  Cr  is  present  in  the  mixture. 
(Goerens,  Metallurgie,  1907,  4.  18.) 


t 

v 

t° 

v 

t° 

v 

0 

0.03287 

7 

0.02796 

14 

0.02466 

1 

0.03207 

8 

0.02739 

15 

0.02432 

2 

0.03131 

9 

0.02686 

16 

0.02402 

3 

0.03057 

10 

0.02635 

17 

0.02374 

4 

0.02987 

11 

0.02588 

18 

0.02350 

5 

0.02920 

12 

0.02544 

13 

0.02329 

6 

0.02857 

13 

0.02504 

20 

0.02312 

Carbon  boride,  CB6. 

Insol.  in  boiling  HNO3+Aq. 
97.  456.) 


(Joly,  C.  R. 


Carbon  sw&oxide,  C3O2. 

B.-pt.+7°  at  761  mm. 

Sol.  in  H2O  with  formation  of  malonic  acid. 

Slowly  decomp.  on  standing  in  a  sealed 
tube.    (Diels,  B.  1906,  39.  696.) 


Carbon  mowoxide,  CO. 

Sol.  in  50  vols.  recently  boiled  H2O.     (Davy.) 
Sol.  in  16  vols.  H2O.     (de  Saussure.) 
Sol.  in  27  vols.  H2O.     (Dalton.) 

100  vols.  H2O  dissolve  6.2  vols.  CO  at  18°.    (de  Saus- 
sure.) 


Solubility  of  CO  in  H2O:  1  vol.  H2O  at  t°  dis- 
solves V  vols.  CO  reduced  to  0°  and  760mm. 


(Bunsen's  Gasometry,  pp.  287,  128,  146.) 


Coefficient  of  absorption : 
0.00081632t +0.000016421 12. 
Pauli,  A.  93.  16.) 


=  0.032874— 
(Bunsen    and 


Solubility  of  CO  in  H2O. 

/3  =  Vol.  CO  absorbed  by  1  vol.  H2O  at  a 
partial  pressure  of  760  mm. 

/3i  =  Vol.  CO  (reduced  to  0°  and  760  mm.) 
absorbed  by  1  vol.  of  H2O  under  a  total  pres- 
sure of  760  mm. 

q  =  g.  CO  dissolved  by  100  g.  H2O  af  a 
total  pressure  of  760  mm. 


t 

P 

31 

q 

0 

0.03537 

0.03516 

0.0044 

5 

0.03149 

0.03122 

0.0039 

10 

0.02816 

0.02782 

0.0035 

15 

0.02543 

0.02501 

0.0031 

20 

0.02319 

0.02266 

0.0028 

25 

0.02142 

0.02076 

0.0026 

30 

0.01998 

0.01915 

0.0024 

40, 

0.01775 

0,01647 

0.0021 

50 

0.01615 

0.01420 

0.0018 

60 

0.01488 

0.01197 

0.0015 

70 

0.01440 

0.00998 

0.0013 

80 

0.01430 

0.00762 

0.0010 

90 

0.01420 

0.00438 

0.0006 

100 

0.01410 

0.00000 

0.0000 

(Winkler,  B.  1901,  34.  1416.) 

CARBON  OXIDE 


159 


Solubility  in  H2O  at  various  pressures. 
V  =  Volume  of  the  absorbing  liquid. 
P  =  Hg  pressure  in  metres. 
X  =  Coefficient  of  solubility. 


Solubility  in  alcohol +Aq. 
%  alcohol 


v 

t° 

p 

A 

30.830  ccm. 

17.7 

0.9202 

0.02791 

1  .  1438 

0.02787 

1  .  4624 

0.02786 

1  .  7986 

0.02783 

2.3659 

0.02782 

2.8390 

0.02776 

3.2622 

0.02771 

4.0114 

0.02770 

' 

4.6017 

0.02763 

5.1953 

0.02761 

.  .  !< 

5.8717 

0.02756 

6.5462 

0.02744 

7.0983 

0.02738 

7.6470 

0.02723 

8.0184 

0.02715 

31.939  ccm. 

19.0 

0.9176 

0.02716 

1  .  1506 

0.02717 

1.3897 

0.02715 

1.7044 

0.02712 

2  1239 

0.02708 

2.7173 

0.02701 

3.2576 

0.02693 

3.9311 

0.02689 

4.4584 

0.02680 

5.2470 

0.02673 

6.0346 

0.02665 

6.6303 

0.02654 

7.1842 

0.02636 

7.9542 

0.02617 

(Cassuto,  Phys.  Zeit.  1904,  5.  236.) 

Coefficient  of  absorption  of  CO  in  H2O  at 
25°  equals  0.0154.  (Findlay  and  Creighton, 
Biochem.  J.  1911,  6.  294.) 

Cuprous  chloride  in  an  hydrochloric  acid  or 
ammoniacal  solution,  and  ammoniacal  solu- 
tions of  cuprous  salts  absorb  large  amounts 
of  CO.  (Leblanc,  C.  R.  30.  488.) 

Cuprous  chloride  dissolved  in  HCl+Aq  ab- 
.sorbs  15-20  vols.  CO.  (Berthelot,  A.  ch.  (3) 
51.  66.) 

Absorbed  by  KOH,  NaOH,  Ba(OH)2,  and 
Ca(OH)2+Aq;  more  readily  by  ether,  alcohol, 
and  wood  spirit,  with  formation  of  formic 
.acid.  (Berthelot,  A.  ch.  (3)  61.  463.) 

Sol.  in  HCN.     (Bottinger,  B.  10.  1122.) 

1  vol.  alcohol  absorbs  0.20443  vols.  CO 
gas  at  all  temperatures  between  0°  and  25°. 
(Carius,  A.  94.  135.) 

100  vols.  alcohol  (0.84  sp.  gr.)  dissolve  14.5  vols.  CO 
at  18°;  100  vols.  rectified  naphtha  (0.784  sp.  gr.),  20.0 
vols.  CO  at  18°;  100  vols.  oil  of  lavender  (0.88  sp.  gr.), 
15.6  vols.  CO  at  18°;  100  vols.  olive  oil  (0.915  sp.  gr.), 
14.2  vols.  CO  at  18°;  100  vols.  sat.  KCl+Aq  (1.168 
sp.  gr.),  5.2  vols.  CO  at  18°.  (de  Saussure,  1814.) 

1  vol.  oil  of  turpentine  absorbs  0.16-0.20  vol.  CO. 
•(de  Saussure.) 

Sol.  in  ether.     (Regnault.) 

Insol.  in  caoutchine. 


by  weight    0.00        9.09         16.67        23.08 

Solubility      2.41         1.87           1.75           1.68 

%  alcohol 

by  weight    28 
Solubility         1 

.57      33.33      50.00 
.50         1.94        3.20 

(Lubarsch,  W.  Ann.  1889,  37.  524.) 

Solubility  of  CO  in  organic  solvents. 

Solvent 

Solubility  at 
20°  C. 

Solubility  at 
25°  C. 

Glycerine 

Not 

measurable 

Water 

0.02404 

0.02586 

Aniline 

0.05358 

0.05055 

Carbon  bisulphide 

0.08314 

0.08112 

Nitrobenzene 

0.09366 

0.09105 

Benzene 

0.1707 

0.1645 

Glacial  acetic  acid 

0.1714 

0.1689 

Amyl  alcohol 

0.1714 

0.1706 

Xylene 

0.1781 

0.1744 

Toluene 

0.1808 

0.1742 

Ethyl  alcohol 

(99.8%) 

0.1921 

0.1901 

Chloroform 

0.1954 

0.1897 

Methyl  alcohol 

0.1955 

0.1830 

Amyl  acetate 

0.2140 

0.2108 

Acetone 

0.2225 

0.2128 

Isobutyl  acetate 

0.2365 

0.2314 

Ethyl  acetate 

0.2516 

0.2419 

(Just,  Z.  phys.  Ch.  1901,  37.  361.) 

Solubility  of  CO  in  ether  at  0°  =  0.3618,  and 

at    10°  =  0.3842.      (Christoff,    Z.    phys.    Ch. 

1912,  79.  459.) 

Solubility  of 

CO  in  organic  mixtures. 

CO  in  benzene  and  naphthalene  at  25°C. 

Per  cent  by  weight 
of  naphthalene 

Per  cent  by  weight 
of  benzene 

*  Solubility  of 
CO 

0 

100 

0.174 

11.52 

88.48 

0.164 

11.65 

88.35 

0.163 

23.98 

76.02 

0.149 

23.60 

76.40 

0.148 

32.35 

67.65 

0.142 

32.74 

67.26 

0.143 

33.79 

66.21 

0.141 

(Skirrow,  Z 

.  phys.  Ch.  1902,  41.  144.) 

*  See  under  Oxygen. 

CO  in  benzene  and  phenanthrene  at  25°  C. 

Per  cent  by  weight 

Per  cent  by  weight 

Solubility  of 

of  phenanthrene 

of  benzene 

CO' 

0 

100 

0.174 

10.48 

89.52 

0.144 

10.48 

89.52 

0.144 

19.22 

80.78 

0.132 

18.99 

81.01 

0.133 

27.04 

72.96 

0.128 

27.39 

72.61 

0.127 

(Skirrow.) 

160 


CARBON  OXIDE 


CO  in  benzene  and  a-naphthol  at  25°  C. 

CO  in  toluene  and  naphthalene  at  25°  C. 

Per  cent  by  weight 
of  a-naphthol 

Per  cent  by  weight 
of  benzene 

Solubility  of 
CO 

Per  cent  by  weight 
of  naphthalene 

Per  cent  by  weight 
of  toluene 

Solubility  of 
CO 

0 
3.48 
6.75 
6.59 
12.10 
11.81 

100 
96.52 
93.25 
93.41 

87.90 

88.19 

0.174 
0.149 
0.145 
0.144 
0.139 
0.139 

0 
7.13 
7.10 
15.10 
15.13 
22.75 
22.58 

100 
92.87 
92.9 

84.9 
84.87 
77.25 

77.42 

0.182 
0.169 
0.171 
0.161 
0.161 
0.153 
0.154 

(Skirrow.) 
CO  in  benzene  and  /S-naphthol  at  25°  C. 

(Skirrow.) 
CO  in  toluene  and  phenanthrene  at  25°  C. 

Per  cent  by  weight 
of  &  naphthol 

Per  cent  by  weight 
of  benzene 

Solubility  of 
CO 

Per  cent  by  weight 
of  phenanthrene 

Per  cent  by  weight 
of  toluene 

Solubility  of 

CO' 

0 
2.06 
4.14 
4.36 

100 
97.94 
95.86 
95.64 

0.174 

0.158 
0.151 
0.149 

0 
5.50 
5.58 
11.16 
11.20 
21.62 
21.93 

100 
94.41 
94.42 

88.84 
88.8 
78.38 
78.07 

0.182 
0.170 
0.171 
0.161 
0.161 
0.147 
0.147 

(Skirrow.) 
CO  in  benzene  and  nitrobenzene  at  25°  C. 

(Skirrow.) 
CO  in  toluene  and  nitrobenzene  at  25°  C. 

Per  cent  by  weight 
of  nitrobenzene 

Per  cent  by  weight 
of  benzene 

Solubility  of 
CO 

Per  cent  by  weight 
of  nitrobenzene 

Per  cent  by  weight 
of  toluene 

Solubility  of 
CO 

0 
14.5 
14.12 
28.18 
28.14 
40.58 
40.63 
54.9 
54.9 
83.33 
83.2 
100 

100 
85.5 
85.88 
71.82 
71.86 
59.42 
59.37 
45.1 
45.1 
16.67 
16.8 
0 

0.174 
0.162 
0.162 
0.152 
0.152 
0.140 
0.140 
0.126 
0.127 
0.101 
0.102 
0.093 

0 

8.86 
8.87 
'     18.27 
18.19 
26.82 
26.76 
49.14 
49.02 
76.31 
76.31 
100 

100 
91.14 
91.13 
81.73 
81.81 
73.18 
73.24 
50.86 
50.98 
23.69 
23.69 
0 

0.182 
0.168 
0.168 
0.160 
0.161 
0.151 
0.151 
0.131 
0.131 
0.108 
0.108 
0.093 

(Skirrow.) 
CO  in  benzene  and  aniline  at  25°  C. 

(Skirrow.) 
CO  in  toluene  and  aniline  at  25°  C. 

Per  cent  by  weight 
of  aniline 

Per  cent  by  weight 
of  benzene 

Solubility  of 
CO 

Per  cent  by  weight 
of  aniline 

Per  cent  by  weight 
of  toluene 

Solubility  of 
CO 

0 
12.69 
12.03 
19.57 
19.43 
28.43 
28.26 
57.68 
57.38 
78.90 
78.80 
100 

100 
87.31 
87.97 
80.43 
80.57 
71.57 
71.74 
42.32 
42.62 
21.10 
21.20 
0 

0.174 
0.156 
0.158 
0.145 
0.144 
0.131 
0.131 
0.0945 
0.0953 
0.0689 
0.0684 
0.053 

0 
6.61 
6.61 
13.56 
13.55 
19.91 
19.96 
44.64 
44.31 
74.63 
75.03 
100 

100 
93.39 
93.39 
86.44 
86.45 
80.09 
80.04 
55.36 
55.69 
25.37 
24.97 
0 

0.182 
0.169 
0.168 
0.157 
0.156 
0.148 
0.148 
0.115 
0.116 
0.0768 
0.0753 
0.053 

(Skirrow.) 

(Skirrow.) 

CARBON  OXIDE 


161 


CO  in  toluene  and  a-naphthol  at  25°  C. 

CO  in  acetic  acid  and  nitrobenzene  at  25°  C. 

Percent  by  weight 
of  a-naphthol 

Percent  by  weight       Solubility  of 
of  toluene                     CO 

Per  cent  by  weight 
of  nitrobenzene 

Per  cent  by  weight    ..,  .  ....        ,  .^^ 
of  acetic  acid        Solubility  of  CO 

0 
4.46 
4.44 

8.75 
8.89 

100                       0.182 
95.54                 0.171 
95.56                 0.171 
91.25                 0.162 
91.11                 0.163 

0 
21.65 
51.03 
100 

100                       0.173 
78.35                 0.156 
48.97                0.130 
0                      0.093 

(Skirrow.) 
CO  in  acetic  acid  and  aniline  at  25°  C. 

(Skirrow.) 
CO  in  acetone  and  naphthalene  at  25°  C. 

Per  cent  by  weight 
of  aniline 

Per  cent  by  weight    „  ,  .... 
of  acetic  acid        Solubility  of  CO 

Per  cent  by 
weight  of 
naphthalene 

Per  cent  by 
weight  of 
acetone 

Measured 
vapor 
pressure 

Solubility 
of  CO 

0 
13.5 
41.64 
60.77 
82.21 
100 

100                      0.173 
86.5                   0.110 
58.36                 0.0699 
39.23                 0.0618 
17.79                0.0580 
0                      0.053 

0 
13.31 
.    27.40 

100 
86.69 
72.60 

229.6 
212.4 
196.6 

0.238 
0.199 
0.187 

(Skirrow.) 
CO  in  acetone  and  phenanthrene  at  25°C. 

(Skirrow.) 
CO  in  methyl  alcohol  and  glycerine  at  25°C. 

Per  cent  by 
weight  of 
glycerine 

Per  cent  by 
weight  of 
methyl 
alcohol 

Measured 
vapor 
pressure 

Solubility 
of  CO 

Percent  by 
weight  of 
phenanthrene 

Percent  by 
weight  of 
acetone 

Measured 
vapor 
pressure 

Solubility 
of  CO 

0 
12.77 
25.04 

100 

87.23 
74.96 

229.6 
218 
207.5 

0.238 
0.205 
0.183 

0 
39.6 
60.5 
77.1 
100 

100 

60.4 
39.5 
22.9 
0 

122 
106 
91 
63 

0.196 
0.0964 
0.0515 
0.0246 
very  small 

(Skirrow.) 
CO  in  acetone  and  /8-naphthol  at  25°  C. 

(Skirrow.) 
CO  in  acetone  and  chloroform  at  25°  C. 

Per  cent  by 
weight  of 
0-naphthol 

Per  cent  by 
weight  of 
acetone 

Measured 
vapor 
pressure 

Solubility 
of  CO 

Per  cent  by 
weight  of 
chloroform 

Per  cent  by 
weight  of 
acetone 

Measured 
vapor 
pressure 

Solubility 
of  CO 

0 

13.95 

26.88 

100 
86.05 
73.12 

229.6 
213 
195 

0.238 

0.190 
0.169 

0 
33.38 
53.2 
65.03 
73.46 
79.83 
87.3 
94.4 
100 

100 
66.62 
46.8 
34.97 
26.54 
20.17 
12.7 
5.6 
0 

229.6 
202 
179 
167 
162 
163 
168 
178 
188 

0.238 
0.226 
0.219 
0.220 
0.212 
0.204 
0.207 
0.205 
0.207 

(Skirrow.) 
CO  in  acetone  and  nitrobenzene  at  25°  C. 

Per  cent  by 
weight  of 
nitrobenzene 

Per  cent  by 
weight  of 
acetone 

Measured 
vapor 
pressure 

Solubility 
of  CO 

0 
21.59 
53.20 
100 

100 

78.4 
46.8 
0 

229.6 
201 
152 

0.238 

0.207 
0.157 
0.093 

(Skirrow.) 
CO  in  acetone  and  carbon  bisulphide  at  25°  C. 

Per  cent  by 
weight  of 
carbon 
bisulphide 

Per  cent  by 
weight  of 
acetone 

Measured 
vapor 
pressure 

Solubility 
of  CO 

(Skirrow.) 
CO  in  acetone  and  aniline  at  25°  C. 

0 

8.18 
18.02 
49.46 
62.6 
74.05 
85.51 
96.42 
100 

100 

91.82 
81.98 
50.54 
37.4 
25.95 
14.49 
3.58 
0 

229.6 
306 
367 
443 
457 
457 
433 
382 
356 

0.238 
0.236, 
0.236- 
0.227 
0.210 
0.187 
0.144 
0.114 
0.0959 

Per  cent  by 
weight  of 
aniline 

Per  cent  by 
weight  of 
acetone 

Measured 
vapor 
pressure 

Solubility 
of  CO 

0 
20.83 
55.10 
100 

100 
79.17 
44.9 
0 

229.6 
192 
120 

0.238 
0.179 
0.110 
0.053 

(Skirrow.) 

(Skirrow.) 

162 


CARBON  OXIDE 


CO  in  benzene  and  ethyl  alcohol  at  25°  C. 

Per  cent  by 
weight  of 
acetic  acid 

Per  cent  by 
weight  of 
chloroform 

Measured 
vapor 
pressure 

Solubility 
of  CO 

0 
15.43 
52.34 
100 

100 
84.56 
47.66 
0 

95.9 
125 
119 
59 

0.174 
0.179 
0.181 
0.192 

(Skirrow.) 
CO  in  chloroform  and  methyl  alcohol  at  25°  C. 

Per  cent  by 
weight  of 
alcohol 

Per  cent  by 
weight  of 
chloroform 

Measured 
vapor 
pressure 

Solubility 
of  CO 

0 
13 

100 

100 
87 
0 

188 
233 
122 

0.207 
0.202 
0.196 

(Skirrow.) 


CO  in  acetic  acid  and  benzene  at  25°  C. 


Percent  by 
weight  of 
acetic  acid 

Percent  bv 
weight  of 
benzene 

Measured 
vapor 
pressure 

Solubility 
of  CO 

0 
19.17 
33.54 
67.51 
100 

100 
80.83 
66.46 
32.49 
0 

95.9 

87.5 
82 
64.5 
14 

0.174 
0.190 
0.198 
0.199 
0.172 

(Skirrow.) 


CO  in  acetic  acid  and  toluene  at  25°  C. 


Per  cent  by 
weight  of 
acetic  acid 

Per  cent  by 
weight  of 
toluene 

Measured 
vapor 
pressure 

Solubility 
of  CO 

0 

20.48 
56.89 
74.71 
100 

100 
79.52 
43.11 
25.29 
0 

9 

31.6 
28 
25.6 
14 

0.182 
0.190 
0.195 
0.191 
0.172 

(Skirrow.) 


CO  in  acetic  acid  and  chloroform  at  25°  C. 


Per  cent  by 
weight  of 
acetic  acid 

Per  cent  by 
weight  of 
chloroform 

Measured 
vapor 
pressure 

Solubility 
of  CO 

0 
26.67 
56.46 
100 

100 
73.33 
43.54 
0 

188 
144.5 
88.5 
14 

0.206 
0.207 
0.196 
0.172 

(Skirrow.) 


CO  in  carbon  bisulohide  and  ethylene  di- 
chloride at  25°  C. 


Per  cent  by 
volume  of 

Per  cent  by 
volume  of 

Measured 

Solubility 

carbon 

bisulphide 

ethylene 
dichloride 

vapor 
pressure 

of  CO' 

0 

100 

77 

0.147 

25 

75 

231 

0.159 

49 

51 

294 

0.160 

81.6 

18.4 

338 

0.140 

100 

.   0 

356.5 

0.083 

(Skirrow.) 

Coefficient  of  absorption  for  petroleum  = 
0.123  at  20°,  and  0.134  at  10°.  (Gniewasz 
and  Walfisz,  Zeit.  phys.  Ch.  1.  70.) 

Carbon  dioxide,  CO2. 
Gas  — 

HzO  dissolves  about  its  own  vol.  CC>2  at  the  ordinary 
temperature  (the  solution  obtained  being  of  1.0018  sp. 
gr.)  and  pressure,  and  an  additional  vol.  for  the  pressure 
of  each  additional  atmosphere  to  which  it  is  subjected. 

The  power  of  H2O  to  absorb  CO2  does  not  increase  in 
precisely  the  same  ratio  as  the  pressure.  (Soubeiran.) 

5  vols.  CO2  dissolve  in  1  vol.  EbO  at  7  atmos.  pressure, 
and  much  greater  pressure  is  necessary  in  order  to  in- 
crease the  amount  of  gas  dissolved;  but  up  to  4  or  5 
atmospheres  the  amount  of  gas  dissolved  is  very  nearly 
proportional  to  the  pressure.  (Courbe,  «L  Pharm.  26. 
121.) 

100  vols.  H2O  at  12.78°  absorb  116  vols.  CO2  (Caven- 
dish); at  29.44°,  84  vols.  CO2  (Henry);  at  15.56°,  106 
vols.  CO2  (Saussure) ;  at  15.56°,  108  vols.  COa  (Henry) ; 
at  15.56°,  100  vols.  CO2  (Dalton). 

100  vols.  H2O  at  t°  C.  absorb  V  vols.  of  CO2  gas 
reduced  to  60°  F.  and  30  in.  pressure. 


0 

4.4 
10 

15.6 
21.1 


175.72 
147 . 94 
122.27 
100.50 
83.86 


26.7 
32.2 
37.8 
65.6 
100 


68.60 
57.50 
50.39 
11.40 
trace 


(Rogers,  Am.  J.  Sci.  (2)  6.  107.) 

1  vol.  H2<D  at  5°  absorbs  somewhat  more  than  1  vol. 
CO2;  at  10°  scarcely  1  vol.,  and  still  less  at  higher  temp. 
CO2-(-Aq  sat.  at  2°  has  1.0015  sp.  gr.;  most  of  the  CO2 
escapes  upon  exposing  the  solution  to  the  air,  the 
more  quickly  the  higher  the  temperature.  But  as  CO2 
diminishes,  the  remainder  is  more  obstinately  held,  so 
that  boiling  for  ^  hour  is  necessary  to  expel  it  com- 
pletely. (Bergman.) 

Solubility  of  CO2  in  H2O.  1  vol.  H2O  at  t° 
and  760  mm.  dissolves  V  vols.  CO2  gas 
reduced  to  0°  and  760  mm. 


.7967 
.7207 
.6481 
.5787 
.5126 
.4497 
1.3901 


7 

8 

9 

10 

11 

12 

13 


.3339 
.2809 
.2311 
.1847 
.1416 
.1018 
.0653 


14 
15 
16 
17 

18 
19 
20 


V44 


1.0321 
1.0020 
0.9753 
0.9519 
0.9318 
0.9150 
0.9014 


(Bunsen's  Gasometry,  pp.  287,  128,  152.) 

Coefficient  of  absorption  =  1.7967 — 0.0776U 
-f-0.0016424t2.    (Bunsen.) 


CARBON  OXIDE 


163 


Solubility  in  H2O  at  various  pressures:  P 
pressure  in  atmospheres. 


Vol.  gas.  in  1  ccm. 

Vol.  gas  in  1  ccm. 

p 

H20 

p 

H20 

at,  0° 

at  12.43° 

at  0° 

at  12.43° 

1 

1.797 

1.086 

20 

26.65 

17.11 

5 

8.65 

5.15 

25 

30.55 

20.31 

10 

16.03 

9.65 

30 

33.74 

23.35 

15 

21.95 

13.63 

-. 

... 

(Wroblewski,  C.  R.  94.  1355.) 

Absorption  of  CO2  in  H2O  at  various  .pres- 
sures: P  =  pressure  in  mm.;  V  =  vols.  CO2, 
reduced  to  0°  and  760°  mm.,  absorbed  by 


Solubility  in  H2O  at  25°  =  0.8255;  at  15°  = 
1.070.  (Geffcken,  Z.  phys.  Ch.  1904,  49.  273.) 

75  cc.  H2O  absorb  0.1381  g.  CO2  at  15.5° 
and  720  mm.  (Christoff,  Z.  phys.  Ch.  1905, 
53.329.) 

Absorption-coefficient  of  CO2  in  H2O  at 
20°  =0.877,  or  1000  g.  H2O  dissolve  878  cc. 
CO2.  (Usher,  Chem.  Soc.  1910,  97.  72.) 

Solubility  of  CO2  in  H2O  =  1.158  at  12°  and 
0.825  at  25°.  (Findlay  and  Shenn,  Chem. 
Soc.  1911,  99.  1315.) 


Absorption  of  CO2  by  H2O  at  high  pressure, 
a  =  0.210  ccm. 


Amount  of  H2O  used 


b=  0.102  ccm. 


1  vol.  H2O. 

V  =  ccm.  of  CO2  absorbed  by  H2O  at  t°,  re- 
duced to  a  pressure  of  1  kg.  per  sq.  cm. 
Vi  =  ccm.  of  CO2  absorbed  by  1  ccm.  of  H2O. 

p 

v 

P                        V 

697.71 
809.03 
1289.41 
1469.95 
2002.06 

0.9441 
1.1619 
1.8647 
2.1623 
2  .  9067 

2188.65          3.1764 
2369.02         3.4857 
2554.  CO         3.7152 
2738.33         4.0031 
3109  51          4.5006 

Pressure 
kg/sq.  cm. 

t 

Vi 

a 

b 

25 
30 
40 
50 
55 

20° 

17.77 
19.77 
21.52 

28.09 
29.75. 

(Khanikoff  and  Longuinine,  A.  ch.   (4)   11. 

412.) 

C  =  coefficient  of  absorption  in  H2O  at  t° 
and  760  mm. 

30 
40 
50 
60 
70 
80 

35° 

11.77 
14.82 
18.96 
22.90 
27.18 

13.57 
20.00 
24.64 
22.50 
27.62 
32.85 

t°             C                t° 

c 

t°            C 

15.2     1.009      18.38 
17.6     0.930      18.3 

0.8P6 

0.885 

21       0  838 
23       0.798 

(Setschenow,   Mem.  Acad.  St.  Petersb.  22. 
Nos.  6,  7.) 

Absorption  coefficient  of  CO2  in  H20  at  0° 
=  1.7308.     (Prytz  and  Hoist,  W.  Ann.  1895, 
54.  136.) 

Absorption  of  CO2  by  H2O  at  t°. 
a  =  coefficient  of  absorption. 

40 
50 
60 
70 
80 
90 
100 
110 
120 

60° 

10.88 
12.24 
14.46 
16.80 
19.74 
22.74 
26.21 
28.92 
30.20 

9.798 
13.72 
15.28 
17.46 
22.67 
21.16 
27.85   • 
28.79 
33.90 

t° 

a 

t° 

a 

0 
1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 

1  713 
1.646 
1.584 
1.527 
1.473 
1.424 
1.377 
1.331 
1.282 
1.237 
1  194 
1.154 
1.117 
1.083 
1.050 
1.019 
0.985 
0.956 
0.928 

19 
20 
21   . 
22 
23 
24 
25 
26 
27 
28 
29 
30 
35 
40 
45 
50 
55 
60 

0  902 
0.878 
0.854 
0.829 
0.804 
0.781 
0.759 
0.738 
0.718 
0  699 
0  682 
0.665 
0.592 
0.530 
0.479 
0.436 
0.394 
0.359 

60 
70 
80 
90 
100 
110 
120 
130 
140 
150 
160 
170 

100° 

8.965 
10.11 
11.05 
12.63 
13.63 
14.88 
16.40 
17.93 
19.56 
20.58 
22.07 
22.78 

6^395 
9.591 
10.85 
12.40 
16.31 
15.78 
16.89 
17.71 
17.49 

(Sander,  Z.  phys.  Ch.  1912,  78.  537.) 

(Bohr,5W.  Ann.  1899,  68.  504.) 

164 


CARBON  OXIDE 


Solubility  of  carbon  dioxide  in  water  at  25°. 

P.  =  Pressure  in  mm.  Hg. 

S.=  Solubility  calculated  according  to  for- 
mula for  which  see  the  original  article. 
(Findlay,  Chem.  Soc.  1910,  97.  538.) 


P 

s 

p 

s 

743 
752 
800 
841 
955 
955 

0.816 
0.817 
0.815 
0.817 
0.816 
0.817 

1059 
1064 
1153 
1243 
1351 
1351 

0.817 
0.819 
0.818 
0.819 
0.820 
0.820 

(Findlay  and  Creighton,  Chem.  Soc.  1910,  97. 
538.) 

Solubility  of  carbon  dioxide  in  water  at  25°; 
P.  =  Pressure  in  mm.  Hg. 
S.=  Solubility.    See  above. 


P 

s' 

p 

s 

755 

0.826 

1069 

0  823 

759 

0.825 

1084 

0.825 

836 

0.825 

1210 

0.825 

841 

0.826 

1211 

0.825 

927 

0.826 

1350 

0.824 

934 

0.824 

1350 

0.826 

Solution 

Grams  CO2  absorbed  by  75  cc. 
at  15.5°  and  720  mm. 

y2-N  H2SO4 

0.1273 

1-N  H2S04 

0.1179 

2-N  H2SO4 

0.1092 

4-N  H2SO4 

0.1003 

(Christoff,  Z.  phys.  Ch.  1905,  53.  329.) 

Solution 

Grams  CO2  absorbed  by  75  cc. 
at  15.5°  and  720  mm. 

2.5%H2SO4 

0.1282 

5% 

0.1179 

10% 

0.0833 

20% 

0.0755 

30% 

0.0751 

40% 

0.0713 

45% 

0.0725 

70% 

0.0918 

90% 

0.1433 

(Christoff,  /.  c.) 

Chem.  Soc.   1912, 


(Findlay  and  Creighton,  C 
101.  1460.) 


Solubility  of  carbon  dioxide  in  water  at  25°. 
P  =  Pressure  in  mm.  Hg. 
S  =  Solubility.    See  above. 


p 

s 

P 

s 

263 
271 
382 
392 
479 

0.817 
0.816 
0.814 
0.811 
0.816 

495 
651 
667 
752 

768 

0.816 
0.816 
0.817 
0.818 
0.817 

(Findlay  and  Creighton,  Chem.  Soc.   1913, 
103.  638.) 

SI.  sol.  in  HCl+Aq. 

100  vols.  H2SO4  of  1.840  sp.  gr.  absorb  45  vols.  CO2. 
(de  Saussure.) 

H2SO4  of  ordinary  density  at  15.56°  and  common 
pressure  absorbs  94%  of  its  vol.  of  CO2;  fuming  H2SO4, 
125%;  the  absorption  for  pure  H2O  under  the  same 
conditions  being  98%.  (Rogers,  Am.  J.  Sci.  (2)  5.  115.) 

H2SO4  absorbs  7-10%  CO2.  (Hlasiwetz, 
W.  A.  B.  20.  193.) 

Coefficient  of  absorption  by  cone.  H2SO4  = 
0.932,  which  is  the  same  as  that  by  H2O;  but 
this  diminishes  on  diluting,  and  is  at  its  lowest 
limit  0.666,  when  the  composition  of  the 
solution  is  H2SO4,  H2O;  upon  further  dilution 
the  coefficient  of  solubility  gradually  increases, 
and  when  58  H2O  are  present  to  1  H2SO4,  the 


coefficient    of    absorption    is    0.857.      (Set- 
schenow,  J.  B.  1876.  46.) 

Absorption  of  CO2  by  H2SO4+Aq. 


Coefficient  of  absorption  for  96%  H2SO4  = 
0.926  at  20.2°.  (Bohr,  Z.  phys.  Ch.  1910,  71. 
48.) 

Absorption  of  CO2  by  acids. 
M  =  Content  in  gram-equivalents  per  liter. 
S  =  Solubility  (see  under  oxygen) . 
Absorption  of  CO2  by  HNO3+Aq. 


M 

825° 

Sl5° 

0.472 

0.8382 

1.073 

0.475 

0.8366 

1.075 

0.557 

0.8387 

1.069 

0.704 

0.8447 

1.080 

1.382 

0.8620 

1.093 

1.387 

0.8622 

1.093 

1.860 

0.8752 

1.105 

2.519 

0.8839 

1.109 

2.539 

0.8865 

1.111 

(Geffcken,  Z.  phys.  Ch.  1904,  49.  273.) 


Absorption  of  CO  £by  HCl+Aq. 


M 

S25° 

Sl5° 

0.499 
0.511 
1.212 
1.249 
2.080 
2.180 

0.8047 
0.8074 
0.7973 
0.7984 
0.7951 
0.7951 

1.041 
1.042 
1.020 
1.023 
0.9864 
1.009 

(Geffcken.) 


CARBON  OXIDE 


165 


Absorption  of  CO2  by 


M 

BM* 

Sl5 

0.512 

0.7923 

1.016 

0.517 

0.7936 

1.016 

0.995 

0.7693 

0.9772 

1.039 

0.7685 

0.9775 

1.067 

0.7672 

0.9756 

1.956 

0.7302 

0.9175 

2.088 

0.7273 

0.9143 

3.790 

0.6736 

0.8354 

3.800 

0.6747 

0.8385 

(Geffcken.) 

In  collecting  COz  gas  in  pneumatic  operations,  a 
saturated  solution  of  common  salt  is  better  than  H2O 
for  filling  the  trough.  This  solution  will  only  absorb 
about  Vs  of  the  amount  of  CO2  absorbed  by  pure  H2O. 
(de  Saussure,  I.  c.) 

100  vols.  of  the  following  solutions  at  18°  and  ordi- 
nary pressure  absorb  vols.  CO2 — 


absorptiometric  equivalents  are  identical  with 
the  chemical  equivalents.  (Setschenow,  B. 
6.  1461.) 

Salts  can  be  divided  into  two  classes,  ac- 
cording as  CO2  has  chemical  action  on  the 
salt  or  not.  In  the  first  case,  i.  e.,  when  there 
is  chemical  combination  or  action  of  CO2  on 
the  salt  in  solution,  the  amount  of  CO2  ab- 
sorbed increases  with  increasing  concentra- 
tion of  the  solution;  in  the  second  case,  how- 
ever, the  amount  of  CO2  decreases  with  the 
strength  of  the  solution.  Several  salts  can 
be  arranged  in  a  series  as  regards  .their  power 
of  absorption,  beginning  with  that  which 
has  the  greatest,  as  follows:  Na2CO3,  Na2B4O7, 
Na2HPO4,  NaC2H3O2,  Na3C6H5O7,  Na2C2O4, 
NaC3HBO3,  MNO3,  MCI,  M2SO4.  The  divi- 
sion between  the  two  classes  occurs  in  this 
series  at  Na2C2O4. 

The  matter  is  discussed  at  length  in  the 
original  papers.  (Setschenow,  Memoires 
Acad.  St.  Petersb.  22.  'No.  3.  Also  further, 


Vols. 

Setschenow,  ib.  34.  No.  3,  and  36.  No.  7. 

Sp.  gr.  CO2 
Sat.  NaCl+Aq  (containing  29%  of  NaCl)    1.212     32.9 
Sat.   NH4Cl+Aq   (containing  27.53%  of 

See  also  Ostwald,   Allgemeine  Chemie,   2fce 
Aufl.  vol.  1,  p.  629.) 

NH4C1)   ...                .                          1  078     75 

Sat.  KCl+Aq  (containing  26%  of  KC1)  .     1.168     61 
Sat.    CaCb+Aq    (containing    40.2%    of 
CaCb)                                                              1  402     26  1 

Solubility  of  CO2  in  salts  +Aq  at  15.2°. 
CO2  =  cc.  CO2.(at  0°  and  760  mm.)  dissolved 

Sat.    K2SO4+Aq    (containing    9.42%    of 
K2SO4)    1.077     62 

per  cc.  of  salt  solution. 

Sat.  Na2SO4+Aq  (containing  11.14%  of 
Na2SO4)  1.105     58 

Salt 

g.  salt  per  1. 

CO2 

Sat.  Iv2Al2(SO4)4+Aq  (containing  9.14% 
of  K2\HSO4)4-f24H2O)                               1047     70 

NH4C1 

1 

1.005 

Sat.    KNOs+Aq    (containing    20.6%    of 

u 

10 

0.985 

KNOs)     1.139     57 

I 

rci    a 

OQ4.1 

Sat.   NaNOs+Aq    (containing  26.4%   of 

( 

Oi.  .  \J 

1  ~.  » 

.  *7TC  J. 

NaNOs)  1.206     45 

1/2 

0.819 

Sat.  H2C4H4O6+Aq  (containing  53.37% 

1 

258 

0.770 

of  H2C4H4O6     T.288     41 

TVTU  T\Tf\ 

20 

1m  Q 

(de  Saussure,  Gilbert's  Ann.  Phys.  47.  167.) 

( 

.«0 

11.2 

.Ulo 

1.002 

About   half   as   sol.    in   NaCl+Aq    (15% 

I 
I 

55 
101 

0.989 
0.962 

NaCl)  as  in  H2O. 

(( 

202.  1 

0.911 

Much    more    sol.    in    Na2HPO4+Aq    or 

(( 

404  *} 

0  SOT 

Na2CO3+Aq  than  in  H2O,  the  quantity  dis- 

(( 

TTV/T:  .  O 

810.4 

\J  .  OVJi 

0.612 

solved  increasing  with  the  amount  of  salt  in 
the  solution.    The  solubility  in  these  solutions 
depends  on  the  coefficient  of  solubility  in  H2O 
plus  the  product  of  a  constant   coefficient 
multiplied  by  the  amount  of  salt  in  the  solu- 

(NH4)2S04 

u 

Ba(N03)2 
Ca(N03)2 
LiCl 

72.2 
144.4 

41. 
16.72 

0.712 
0.575 
0.922 
0.923 
1.035 

tion;  this  constant  equals  0.069  for  Na2HPO4, 

50.  15 

0  808 

and  0.088  for  N  a2CO3.    (Fernet,  A.  ch.  (3)  47. 

« 

125.4 

0.596 

307.) 

u 

250.8 

0.497 

Fernet's  determinations  are  not  accurate. 

f( 

501  5 

0  120 

(L.  Meyer,  A.  Suppl.  2.  157.) 
I    mol.    Na2HPO4   in   dil.    Na2HPO4+Aq 

MgS04 

H 

26^5 
79.5 

0/901 
0.669 

absorbs  2  mols.  CO2.    (Setschenow.) 

it 

159 

0^441 

Solutions  of  salts  of  similar  constitution  are 

(( 

318. 

0  188 

equivalent  in  regard  to  their  power  of  absorp- 
tion of  CO2,  when  they  contain  the  same  per- 

KBr 

83^9 
167  7 

0'908 
0  819 

centage  of  crystal  water.    Experiments  were 
made  with  solutions  of  alum,  MgSO4,  7H2O, 

" 

251.5 
503  .  1 

0.748 
0.579 

and  ZnSO4,   7H2O,   containing  10%  of  the 
salts.      The   MgSO4   solution   absorbed   the 

KI 

319^1 

478.6 

0.777 
0.688 

greatest  proportional  amount  of  CO2,   and 

H 

957.3 

0.506 

the  alum  the  least.    The  further  rule  was  de- 

KSCN 

326 

0.691 

duced  that  with  salts  of  similar  constitution 

u 

489 

0.590 

and  the  same  amount  of  crystal  water,  the 

166 


CARBON  OXIDE 


Solubility  of  CO2  in  salts  +Aq  at  15.2°—  Cont. 

Absorption  of  CO2  by  CsCl+Aq. 
M  =  Content  in  g.  equiv.  per  1. 
S  =  Solubility.    (See  under  Oxygen.) 

Salt 

g.  salt  per  1. 

C02 

KSCN 
KNO3 

u 

NaCl 

u 

n 
u 

NaBr 
v 

NaNO3 
u 

u 
a 
tt 

NaC103 

u 

Na2SO4 

a 

n 

ZnSO4 

n 

(i 
« 

978 
58.8 
117.5 
235.1 
12.9 
64 
128 
192 
115.1 
460.3 
690.4 
89.3 
125 
208.4 
416.8 
625.2 
233.3 
349.9 
699.8 
14,2 
94.8 
284.4 
38.3 
76.7 
230. 
460 

0.387 
0.959 
0.890 
0.781 
0.978 
0.760 
0.580 
0.466 
0.775 
0.364 
0.221 
0.835 
0.762 
0.621 
0.385 
0.244 
0.625 
0.506 
0.257 
0.950 
0.620 
0.234 
0.903 
0.783 
0.474 
0.209 

M 

S25° 

Slo° 

0.552 
0.554 

'0.7771 
0.7769 

1.001 
0.9995 

(Geffcken,  Z.  phys.  Ch.  1904,  49.  273.) 
Absorption  of  C02  by  KNO3+Aq. 

M 

S23° 

Sl5° 

0.536 
0.537 
1.022 
1.033 

0.7832 
0.7818 
0.7452 
0.7447 

1.002 
0.9997 
0.9439 
0.9421 

(Geffcken.) 
Absorption  of  CO2  by  KI+Aq. 

M 

S2o° 

Si5° 

0.559 
0.573 
1.043 
1.119 

0.7678 
0.7676 
0.7236 
0.7166 

0,9809 
0.9835 
0.9144 
0.9090 

(Setschenow,  A.  ch.  1892,  (6)  26.  226.) 

CO2  is  not  disengaged  at  ordinary  temp, 
from  H2O,  in  which  Vmoo  pt.  of  CaCO3  or 
MgCO3  is  held  in  solution  thereby.  These 
solutions  have  a  great  power  of  retaining  CO2 
even  at  a  boiling  temp,  or  with  diminished 
pressure,  and  they  also  absorb  CO2  from  the 
air  in  much  larger  quantity  than  pure  H2O. 
(Bineau.) 

BaCO3  in  H2O  also  retains  CO2  even  after 
long  boiling.  (Storer.) 

CO2   is   also    absorbed   from    the   air   by 
Na2CO3,  or  K2CO3+Aq,  especially  if  dilute. 
Absorption  of  CO2  by  NaCl+Aq  at  t°. 

a  =  Coefficient  of  absorption  for  a  6.52% 
NaCl  solution. 

a,  =  Coefficient  of  absorption  for  a  17.62% 
NaCl  solution. 


t° 

a 

ai 

0 

1.234 

0.678 

5 

1.024 

0.577 

10 

0.875 

0.503 

15 

0.755 

0.442 

20 

0.664 

0.393 

25 

0.583 

0.352 

30 

0.517 

0.319 

35 

0.460 

0.288 

40 

0.414 

0.263 

45 

0.370 

0.235 

50 

0.335 

0.215 

55 

0.305 

0.198 

60 

0.183 

(Bohr,  W.  Ann.  1899,  68.  504.) 


(Geffcken.) 


Absorption  of  CO2  by  RbCl+Aq. 


M 

S25° 

Sl5° 

0.479 
0.481 
1.007 
1.012 

0.7705 
0.7698 
0.7190 
0.7157 

0.9908 
0.9910 
0.9210 
0.9200 

(Geffcken.) 


Absorption  of  CO2  by  KBr+Aq. 


M 

S25° 

Su°     ' 

0.550 
0.565 
1.056 
1.064 

0.7621 
0.7619 
0.7030 
0.7068 

0.9783 
0.9766 
0.9100 
0.9065 

(Geffcken.) 
Absorption  oj  CO2  by  KCl+Aq. 

M 

S25° 

Slo° 

'  0.423 
0.432 
1.045 
1.058 

0.7695 
0.7667 
0.6920 
0.6961 

0.9892 
0.9865 

0.8875 
0.8910 

(Geffcken.) 

CARBON  OXIDE 


167 


Absorption  of  CO2  by  salts  +Aq. 

Solubility  of  C02  in  NH4Cl+Aq  at  25°. 
Concentration    (C)    denotes    number    of 
grams  of  solute  in  100  cc.  of  solution. 
Density  (D)  equals  the  specific  gravity  of 
the  solution. 
Solubility  (S)  calculated  by  formula  given 
in  the  original  article. 

Salt 

Grams  CO2  absorbed  by  7o 
cc.  of  salt  solution  at  15.5 
and  720  mm. 

1-N  KBr 
1-N  KNO3 
1-N  KC1 

0.1280 
0.1231 
0.1213 
0.1204 
0.1087 
0.1050 
0.1093 

0.0991 
0.1002 

0.1054 
0.1140 
0.1209 
0.1047 
0.0656 
0.0527 
0.0751 
0.0720 
0.1017 
0.0999 
0.0808 
0.0852 
0.1111 
0.4989 
0.2205 
0.5317 
0.8511 
0.8124 
0.7672 
0.5828 
0.8457 
0.2081 
0.2618 

1-N  KI 
1-N  LiCl 
1-N  NaCl 
1-N  (NH4)2SO4 
1-N  (NH4)2S04, 
Fe2SO4)3+24H2O 
1-N  K2S04 
1-N  K2SO4, 
Al2(SO4)3+24HoO 
2/3-N  K2SO4 
Vr-N  MgS04 
l-N  MgSO4 
2-N  MgSO4 
4-N  Mo^O 

C 

D 

S 

2.35 
5.05 
8.24 
10.02 
17.09 

1.005 
1.013 
1.022 
1.027 
1.045 

0.791 
0.754 
0.732 
0.712 
•  0.665 

(Findlay  and  Shenn,  Chem. 
Soc.  1912,  101.  1461.) 

Solubility  of  CO2  in  KCl+Aq  at  25°. 

C 

D 

S 

2-N  CuSO4 
2-N  ZnSO4 
2/3-N  KHSO3 
2-N  KHS04 
1-N  KH2As04 
1-N  KH2PO4 
V2-N  K2HAsO, 
1/2-N  K2HP04 
'Ao-N  Na2B407 
Vr-N  Na2B407 
i/4-N  Na2B4O7 
i/4-N  NaBO3 
V4-N  NH4HB2O4 
N-Na2PO4  +  12H2O 
N-Na4P2O7  +  10H2O 
N-NaPOa 
N-KPO3 

1.84 
3.05 
4.58 
7.46 

1.008 
1.017 
1.026 
1.044 

0.792 
0.764 
0.749 
0.701 

(Findlay  and  Shenn.) 
Solubility  of  CO2  in  BaCl2-(-Aq  at  25°. 

C 

D 

S 

2.80 
5.81 
8.15 
9.97 

1.018 
1.040 
1.054 
1.070 

0.789 
0.741 
0.710 
0.676 

(Findlay  and  Shenn.) 

Solubility  of  CO2  in  (NH4)2Fe(SO4)2+Aq  at 
25°. 

(Christoff,  Z.  phys.  Ch.  1905,  53.  338-340.) 

Solubility  of  CO2  in  KCl+Aq  at  25°. 
Concentration,  7.45  g.  in  100  cc.  of  solu- 
tion, sp.  gr.  =  1.043. 

Pressure     756     850     953     1116   1249   1362 
Solubility  0.694  0.693  0.688  0.700  0.709  0.710 

Concentration,  5  g.  in  100  cc.  of  solution, 
sp.  gr.  =  1.031. 

Pressure     756     832     901      1050   1150  1223 
Solubility  0.731  0.727  0.724  0.726  0.735  0.736 

Concentration,  2.56  g.  in  100  cc.  of  solution, 
Sp.  gr.  =  1.016. 

Pressure     756     852     981    1079     1190  1362 
Solubility  0.767  0.761  0.761  0.762  0.768  0.766 
(Findlay  and  Creighton,   Chem.   Soc.   1910, 
97.  557.) 

C 

D 

S 

9.51 
10.26 
22.47 

1.052 
1.057 
1.124 

0.641 
0.629 
0.460 

(Findlay  and  Shenn.) 

Solubility  of  CO2  in  solutions  of  sucrose  at 
25°. 

C 

D 

S 

2.63 
5.16 
9.68 
12.33 

1.009 
1.018 
1.038 
1.051 

0.813 
0.798 
0.767 
0.744 

(Findlay  and  Shenn.) 

Solubility  of  CO2  in  solutions  of  chloral  hy- 
drate at  25°. 

C 

D 

S 

5.08 
10.12 

1.019 
1.041 

0.815 
0.795 

(Findlay  and  Shenn.) 

168 


CARBON  OXIDE 


100  vols.  alcohol  (0.803  sp.  gr.)  at  18°  absorb  260 
vols.  CO2. 

100  vols.  alcohol  (0.840  sp.  gr.)  at  18°  absorb  186 
vols.  COs.  (de  Saussure,  I.  c.) 


Solubility  of  CO2  in  alcohol.  1  vol.  alcohol 
at  t°  and  760  mm.  dissolves  V  vols/  CO2 
gas  reduced  to  0°  and  760  mm. 


t° 

V 

t° 

V 

t° 

V 

0 

4.3295 

9 

3.5844 

18 

3.0402 

1 

4.2368 

10 

3.5140 

19 

2.9921 

2 

4.1466 

11 

3.4461 

20 

2.9465 

3 

4.0589 

12 

3.3807 

21 

2.9034 

4 

3.9736 

13 

3.3178 

22 

2.8628 

5 

3.8908 

14 

3.2573 

23 

2.8247 

6 

3.8105 

15 

3.1993 

24 

2.7890 

7 

3.7327 

16 

3.1438 

8 

3.6573 

17 

3  .  0908 



(Bunsen's  Gasometry,  pp.  287,  128,  153.) 


Coefficient    of    absorption  =4. 32955 — 
0.09395t+0.00124t2.    (Bunsen.) 


Much  less  sol.  in  30%  alcohol  than  in  pure 
alcohol  or  pure  H2O.     (Miiller,  W.  Ann.  37. 

24.) 


Solubility  of  CO2  in  99%  alcohol  at  t°. 

a  =  Coefficient  of  absorption,  i.  e.,  the  no. 
of  ccm.  of  CO2  measured  at  0°  and  760  mm. 
which  are  absorbed  at  the  given  temp,  and 
at  an  absorption  pressure  of  760  mm.  by 
1  ccm.  alcohol. 

a!  =  Coefficient  of  absorption  corrected  for 
increase  in  the  volume  of  the  alcohol  used  due 
to  absorption  of  CO2. 


t° 

a 

<*i 

0 
—10 
—20 
—30 
—40 
—50 
—60 
—65 
—67 

4.35 
5.43 
7.25 
9.97 
14.25 
21.28 
31.25 
39.89 
44.07 

4.31 
5.38 
7.16 
9.79 
13.89 
20.49 
29.59 
37.22 
40.83 

(Bohr,  W.  Ann.  1900,  (4)  1.  253.) 
Solubility  in  alcohol  +Aq  at  t°. 

t 

%  by  wt.  of 
alcohol  in  the 
solvent 

Solubility  of        ~ 
PO,  in             Solubility  of 

\^\J2  in                     /-^/-\     •       TT  r 

alcohol  +Aq 

1 
3 
9 
13 

4         6.325 
2         4.464 
2         7.276 

8         2.870 

1.5864             1.6916 
1  .  4878             1  .  5652 
1.1829             1.2216 
1.0268             1.0385 

t° 

a 

«i 

—65 

38.41 

35.93 

—25 

8.75 

8.61 

—20 

7.51 

7.41 

—15 

6.59 

6.51 

—10 

5.75 

5.69 

—5 

5.01 

4.96 

0 

4.44 

4.40 

+5 

3.96 

3.93 

10 

3.57 

3.55 

15 

3.25 

3.23 

20 

2.98 

2.96 

25 

2.76 

2.74 

30 

2.57 

2.56 

35 

2.41 

2.39 

40 

2.20 

2.19 

45 

2.01 

2.00 

(Bohr,  W.  Ann.  1900,  (4)  1.  249.) 

a  =  Coefficient  of  absorption. 

0!=  Coefficient  of  absorption  corrected  for 
increase  in  volume  of  the  alcohol  used  due  to 
absorption  of  CO2. 


(Langer,  C.  C.  1904,  I,  1583.) 


Solubility  of  CO2  in  ethyl  alcohol  at  25°. 

Concentration.     2.95  g.  alcohol  in  100  cc. 
of  solution.    Sp.  gr.  25°/15°  =  0.99308. 
Pressure     737     836     929     1073   1213    1338 
Solubility  0.812  0.813  0.812  0.811  0.813  0.811 


Concentration.    3.01  g.  alcohol  in  100  cc. 
of  solution.    Sp.  gr.  25°/15°  =0.99295. 
Pressure     745     823     937     1083    1226    1357 
Solubility  0.814  0.812  0.815  0.813  0.812  0.812 


Concentration.  8.83  g.  alcohol  in  100  cc. 
of  solution.  Sp.  gr.  25°/l 5°  =0.98342. 
Pressure  747  846  942  1090  1231  1360 
Solubility  0.786  0.786  0.784  0.785  0.786  0.788 
(Findlay  and  Shenn,  Chem.  Soc.  1911.  99. 
1315.) 

Solubility  of  CO2  in  organic  solvents  at  low 

temperatures. 
Solvent.     Ethyl  alcohol.. 


t  =—78°;  sp.  gr.  =0.872 


Pressure 

Coefficient  of 
absorption 

Solubility 

100 

200 
400 
700 

111.8 
115.7 
123.8 
138.6 

68.4 

69.5 
71.4 
74.7 

CARBON  OXIDE 


169 


Solubility  of  CO->  in  organic  solvents  at  low 
temperatures.  —  Continued 

Solubility  of  Co2  in  organic  solvents  at  low 
temperatures.  —  Continued 

t=—  59°;sp.  gr.  =0.856 

t=—  59°;  sp.  gr.  =0.994 

Pressure 

Coefficient  of 
absorption 

Solubility 

Pressure 

Coefficient  of 
absorption 

Solubility 

100 
200 
400 
700 

40.85 
41.00 
42.35 
44.15 

27.27 
27.16- 
27.65 
28.10 

100 
200      - 
400 
700 

85.3 
86.3 
91.6 
101.5 

65.6 
65.3 
66.7 
69.7 

Solvent.     Methyl  alcohol. 

Solvent.     Methyl  acetate. 

t=—  78°:  So.  er.   =0.884 

Pressure 

Coefficient  of 
absorption 

Solubility 

t  =  —  78°;  sp.  gr.  =1.056 

Pressure 

Coefficient  of 
absorption 

Solubility 

50 
100 
200 
400 
500 
740 

194.0 
195.0 
202.9 
221.5 
226.4 
260.0 

120.5 
119  6 
120.1 
122.2 

126.'  8 

50 
100 
200 
400 
650 

304.9 
315.0 
337.4 
389  3 
498.1 

224.1 
224.3 
223.1 
225.6 
231.2 

t°=  59°;sp.gr.=  0.866 

t—      59°  •  sp   gr  —  1  ( 

)32 

Pressure 

Coefficient  of 
absorption 

Solubility 

Pressure 

Coefficient  of 
absorption 

Solubility 

100 
200 
400 
700 

63.0 
64.2 
66.3 
69.0 

42.5         ' 

42.7 
43.1 
43.3 

100 
200 
400 

700 

94.3 
98.45 
103.6 
112.9 

75.8 

77.1 
77.6 
79.0 

Solvent.     Acetone. 

(Stern,  Z.  phys.  Ch.  1912 

Solubility  of  CO2  in  ether 
10°  =6.044;  at  15°  =  5.46.    (Ch 
Ch.  1912.  79.  459.) 
Coefficient  of  absorption  ii 
0.20376  at  36.57  mm.,  and  4.4< 
pressure.    (Woukoloff,  C.  R. 

100  vols.  of  following  liquids  absor 
Ether  

5,  81.  468.) 

at  0°  =  7.33;  at 
iristoff,  Z.  phys. 

i  chloroform  is 
J757  at  762  mm. 
L09.  62.) 

)  vols.  CO2  at  18°— 
Sp.  gr.     Vols.  CO  2 
0.727            217 
0.784             169 
0.860            166 
0.880            191 
0.890            188 
0.940             156 
0.915             151 

1  .  092              75 
1.104              72 

t=—  78°;  sp.gr.  =0.900 

Pressure 

Coefficient  of 
absorption 

Solubility 

50 
100 
200 
400 
640 
700 

311 
322 
344.5 
400 

487 
545.5 

196.6 
198.1 
201.5 

208.8 
215.7 

t=—  59°;  sp.gr.  =0.879 

Rectified  napht 
Oil  of  turpentii 
Oil  of  lavender 
Oil  of  thyme 

ie    .     .     .     .     .     . 

(freshly  distilled)  . 

Pressure 

Coefficient  of 
absorption 

Solubility 

Olive  oil    .     . 
Gum-arabic  +1 
of  the  gum) 
Cane  -sugar  -f-  A 

100 
200 
460 
700 

.97.8 
101.2 
106.6 

118.8 

67.2 
68.0 

72.8 

72.8 

Iq  (containing  25% 
q  (containing  25% 

(de  Saussure,  I.  c.) 
1  vol.  oil  of  turpentine  absorbs  1.7-1.9  vols.  COi 

1  vol.  spirit  at  10°  absorbs  2  vols.  COz.    (de  Saussure.) 
1  vol.  olive  oil  at  10°  absorbs  1  +vol.  CO».     (de  Saus- 

1  vol.  oil  of  turpentine  at  10°  absorbs  2  vols.  COz. 
"Tvo!.  caoutchine  absorbs  11  vols.  COz.     (Bergman.) 

Coefficient  of  absorption  for  petroleum  is 
1  17  at  20°  and  1.31  at  10°.     (Gniewasz  and 
Walfisz,  Zeit.  phys.  Ch.  1.  70.) 
100  vols.  petroleum  absorb  70  vols.  CO2  at 
10°.     (Robinet,  C.  R.  58.  608.) 

Solvent.  —  Ethyl  acetate. 

t=—  78°;  sp.  gr.  =1.017 

Pressure 

Coefficient  of 
absorption 

Solubility 

50 
100 
200 
400 
650 

250.2 
255.6 
271.8 
310.9 
386.9 

177.5 
177.1 
179.2 
183.2 
191.2 

170 


CARBON  OXIDE 


N 
Solubility  of  CO2  in  —  solutions  of  various 

organic  substances  at  20°. 

Absorption  of  C02  by  propyl  alcohol. 
Amount  of  alcohol  used  =  0.103  ccm. 
V  and  Vi.     See  under  absorption  of  CO2 
by  ethyl  alcohol. 

Substance 

Sp.  gr.  of 
—  solution 

~     _     ,     cc.  CO2 
Coeff.  of    dissolved 
absorp-       m  JQQO 
tion          g.  H20 

Pressure 
kg/sq.cm. 

t° 

Gas  volume 
ccm. 

v 

Vi 

20 
30 
40 
50 

20° 

60.59 

4.867 
8.472 
13.46 
21.62 

56.16 
86.62 
122.1 
174.6 

Dextrose 
Mannite 
Glycerine 
Pyrogallol 
Hydrochinon 
Resorcin 
Pyrocatechin 
Urethane 
Carbamide 
Thio  carbamide 
Antipyrine 
Acetamide 
Acetic  acid 
N  .  Propylic  acid 

1.0328 
1.03031 
1.01413 
1.01718 
1.00946 
1.00958 
1.0107 
1.0037 
1.00715 
1.00917 
1.01339 
1.005 
1.0026 
0.9939 

0.792       841 
0.782       833 
0.843       864 
0.853       894 
0  887       928 
0.901        945 
0.868       908 
0.869       907 
0.864       884 
0.859       885 
0.859       935 
0.879       906 
0.868       893 
0.869       902 

20 
30 
40 
50 
60 
70 
80 

35° 

62.96 

3.493 
6.307 
9.296 
13.99 
18.90 
35.03 
49.23 

40.00 
64.08 
98.16 
122.8 
159.9 
228.2 
269.6 

20 
30 
40 
50 
60 
70 
80 
90 
100 

60° 

68.08 

2.602 
4.722 
6.723 
9.810 
13.05 
17.15 
19.61 
24.75 
30  19 

24.73 
47.68 
64.65 
88.54 
111.5 
144.4 
159.2 
184.3 
213  9 

(Usher,  Chem.  Soc.  1910,  97.  73.) 

Absorption  of  CO2  by  ethyl  alcohol. 

Amount  of  alcohol  used  =0.093  ccm. 
V  =  ccm.  of  CO2  absorbed  by  the  solvent 
at  t°,  reduced  to  a  pressure  of  1  kg.  per  sq.  cm. 
Vi  =  ccm.  of  CO2  absorbed  by  1  ccm.  of  the 
solvent. 

40 
50 
60 
70 
80 
90 
100 
110 
120 

100° 

76.27 

2  592 
5.669 
8.025 
10.44 
13.13 
15.72 
17.10 
20.95 
23.55 

26  50 
54.19 
74.51 
92.17 
107.7 
132.3 
144.7 
163.5 
175.4 

Pressure 
kg/sq.cm. 

t° 

Gas  volume  1 
ccm. 

V 

Vi 

30 
40 
50    ' 

20° 

57.31 

9.462 
15.15 
23.04 

104.8 
149.7 

188.8 

30 
40 
50 
60 
70 

35° 

60.05 

7.114 
10.52 
14.73 
19.63 
27.39 

77.87 
113.1 
144.5 
173.0 
210.8 

(Sander.) 

Absorption  of  CO2  by  ether. 
Amount  of  ether  used  =  0.131  ccm. 
V  and  Vi.     See  under  absorption  of  CO2 
by  alcohol. 

40 
50 
60 
70 
80 
90 
100 

60° 

64.44 

6.429 
9.023 
12.27 
15.64 
19.11 
20.64 
23.88 

72.82 
97.09 
122.5 
145.2 
167.9 
180.7 
195.7 

Pressure 
kg/sq.cm. 

t° 

Gas  volume 
ccm. 

v 

Vt 

45 

50 
60 

35° 

62.06 

42.62 
46.81 
57.83 

205.6 
217.3 
241.6 

50 
60 
70 
80 
90 
100 

60° 

67.11 

28.49 
35.24 
42.01 
46.64 
50.72 
56.63 

171.6 
195.4 
210.0 
221  A 
235.0 
248.7 

50 
60 
70 
80 
90 
100 
110 
120 
130 
140 

100° 

72.19 

3.809 
6.034 
8.374 
10.76 
13.06 
14.90 
16.22 
18.93 
20.48 
20.61 

42  .49 
66.05 
88.67 
111.2 
129.0 
145.7 
155.0 
174.6 
182.6 
186.0 

60 
70 
80 
90 
100 

100° 

71.03 

12.57 
20.00 
26.34 
32.16 
35.70 

101.0 
134.6 
142.8 
166.4 
175.4 

(Sander,  Z.  phys.  Ch.  1912,  78.  524.) 

(Sander.) 

CARBON  OXIDE 


171 


Absorption  of  CO2  by  benzene. 
Amount  of  benzene  used  =  0.080  ccm. 
V  and  Vi.    See  under  absorption  of  CO2  by 
ethyl  alcohol. 

Absorption  of  CO2  by  chlorbenzene.  —  Cont. 

Pressure 
kg/sq.cm. 

t° 

Gas  volume 
ccm. 

V 

Vi 

50 
60 
70 
80 
90 
110 

11.16 
13.74 
16.65 
19.50 
22.23 
31.64 

99.06 
118.1 
134.5 
149.3 
165.5 
204.4 

Pressure 
kg/sq.cm. 

t° 

Gas  volume 
ccm. 

v 

Vi 

15 
20 
30 
40 

50 

20° 

55.14 

2.728 
4.845 
9.618 
18.70 
30.10 

46.89 
71  16 
125.3 
192.4 
264.3 

30 
40 
50 
60 
70 
80 
90 
100 
110 
120 
130 

100° 

77.73 

3.562 
5.008 
7.106 
8.701 
10.37 
12.05 
13.88 
14.89 
16.35 
17.77 
18.54 

33.65 
48.16 
63.78 
77.24 
91.02 
103.00 
121.2 
121.5 
130.7 
140.7 
146.8 

15 
20 
30 
40 
50 
60 
70 

35° 

58.17 

2.225 
3.373 
6.879 
11.56 
17.09 
25.73 
35.80 

39.94 
48.65 
94.39 
138.3 
186.6 
243.1 
269.0 

20 
30 
40 
50 
60 
70 
80 
90 
100 

60° 

61.86 

2.140 
3.880 
6.699 
10.28 
13.57 
17.71 
22.50 
28.09 
33.76 

34.57 
55.97 
88.71 
128.5 
156.6 
1*84.6 
215.0 
246.6 
284.4 

(Sander.) 
Absorption  of  CO2  by  brombenzene. 
Amount  of  brombenzene  used  =  0.1  13  ccm. 
V  and  Vi.     See  under  absorption  of  CO2 
by  ethyl  alcohol. 

Pressure 
kg/sq.cm- 

t° 

Gas  volume 
ccm.    • 

V 

V, 

20 
30 
40 
50 

20° 

60.84 

4.531 
7.793 
12.22 
17.37 

50.83 
82.29 
121.1 
160.0 

40 
50 
60 
70 
80 
90 
100 
110 
120 

100° 

73.75 

2.822 
3.981 
6.440 
8.398 
11.96 
14.57 
17.79 
20.60  • 
23.98 

46.52 
58.46 
91.27 
119.0 
155.8 
182.5 
212.9 
•237.7 
258.2 

20 
30 
40 
50 
60 
70 
80 

35° 

63.96 

3.947 
5.782 
8.508 
11.96 
16.00 
22.56 
41.26 

43.38 
62.69 
90.43 
116.4 
146.0 
184.1 
233.9 

(Sander.) 

Absorption  of  CO2  by  chlorbenzene. 
Amount  of  chlorbenzene  used  =  0.106  ccm. 
V  and  Vi.    See  under  absorption  of  CO2  by 
ethyl  alcohol. 

20 
30 
40 
50 
60 
70 
80 
90 
100 
110 

60° 

69.16 

2.650 
3.714 
5.971 
7.406 
9.718 
10.27 
13.99 
16.76 
20.06 
23.13 

30.58 
46.15 
62.64 
77.19 
98.73 
108.4 
131.4 
144.3 
169.7 
190.6 

Pressure 
kg/sq.cm. 

t° 

Gas  volume 
ccm. 

v 

Vi 

20 
30 
40 
50 

20° 

61.03 

5.813 
10.25 
17.17 
26.59 

62.61 
95.22 
137.3 
187.5 

30 
40 
50 
60 
70 
.  80 
90 
100 
110 
120 

100° 

77.48 

2.970 
4.032 
5.833 
7  239 
8.330 
9.714 
11.14 
12.79 
13.80 
15.50 

30.56 
41.49 
59.64 
72.64 
82.56 
92.86 
107.1 
118.0 
125.3 
140.7 

20 
30 
40 
50 
60 
70 

35° 

64.16 

4.650 
7.705 
11.81 
16.83 

22.82 
32.83 

46.66 
72.73 
101.5 
137.3 
168.3 
205.5 

20 
30 
40 

60° 

69.38 

3.685 
5.510 

7.982 

35.86 
53.94 
73.69 

(Sander.) 

172 


CARBON  OXIDE 


Absorption  of  CO2  by  nitrobenzene. 
Amount  of  nitrobenzene  used  =0.164  com. 
V  and  Vi.     See  under  absorption  of  CO2 
by  ethyl  alcohol. 

Absorption  of  CO2  by  toluene.  —  'Continued 

Pressure 
kg/sq.cm. 

t° 

Gas  volume 
ccm. 

'  V 

Vi 

30 
40 
50 
60 
70 
80 
90 
100 
110 
120 
130 

100° 

76.37 

3.356 
5.945 
8.703 
11.18 
13.72 
16.30 
18-.  88 
21.85 
24.86 
26.80 
28.21 

28.68 
49.25 
67.93 
85.98 
101.7 
117.6 
132.6 
149.0 
161.9 
171.8 
178.7 

Pressure 
kg/sq.cm. 

t° 

Gas  volume 
ccm. 

v 

Vi 

15 
20 
30 
40 
50 

20° 

57.65 

5.459 
7.354 
12.14 
15.93 
21.71 

41.60 
57.12 
92.50 
115.9 
155.9 

20 
30 
40 
50 
60 
70 
80 

35° 

59.86 

5.644 
8.658 
11.98 
15.59 
19.94 
25.57 
34.95 

44.48 
68.23 
94.39 
113.4 
145.1 
179.6 
227.0 

(Sander 

Absorption  of  CO2  bj 
Amount  of  ethyl  acetat 
V  and  Vi.     See  under 
by  ethyl  alcohol. 

) 

'  ethyl  ace 
e  used  ~  0 

tate. 
.155  ccm. 
n  of  CO2 

20 
30 
40 
50 
60 
70 
80 

60° 

64.73 

3.787 
4.519 
6.308 
7.750 
8.887 
10.15 
10.80 

31.38 
38.23 
52.26 
64.21 
72.15 
82.40 
85.03 

absorptio 

Pressure 
kg/sq.cm. 

t° 

Gas  volume 
ccm. 

V 

Vi 

25* 
30* 
40 

20° 

60.30 

29.43 
37.91 
51.26 

158.6 
188.2 
227.9 

20 
30 
40 
50 
60 
70 
80 

100° 

75.52 

2.749 
4.162 
5.393 
6.832 
7.763 
9.048 
10.65 

24.67 
41.00 
50.36 
63.80 
70.85 
75.75 
86.86 

30 
40 
50 
60 

35° 

63.40 

26.54 
38.69 
48.35 
51.88 

145.2 

188.4 
213.9 
219.8 

30 
40 
50 
60   • 
70    , 
80 

60° 

• 

68.55 

18.12 
25.67 
33.21 
40.12 
45.47 
49.16 

108.0 
110.5 
165.2 
186.7 
201.1 
223.4 

(Sander.) 
Absorption  of  CO2  by  toluene. 
Amount  of  toluene  used  =0.114  ccm. 
V  and  VL     See  under  absorption  of  CO2 
by  ethyl  alcohol. 

40 
50 
60 
70 
80 
90 
100 

100° 

76.80 

12.76 
18.80 
24.12 
28.99 
32.96 
36.92 
42.75 

80.70 
110.1 
132.0 
152.0 
162.3 
172.1 
191.5 

Pressure 
kg/sq.cm' 

t° 

Gas  volume 
ccm. 

V 

Vi 

20 
30 
40 
50 

20° 

59.97 

7.420 
13.31 
23.25 
45.10 

57.91 
103.3 
155.9 

235.8 

20 
30 
40 
50 
60 
70 

30 
40 
50 
60 
70 
80 
90 
100 

35° 

63.05 

6.018 
10.13 
16.03 
23.34 
31.39 
44.17 

49.60 
82.63 
118.8 
155.8 
192.1 
225.8 

(Sander.) 
Absorption  of  CO2  by  CH3COOH+CC14. 

Solvent 

cc.  CO2  absorbed 

1      mol.  CH3COOH 
0.8           CH3COOH  + 
0.2           CC14 
0.5          CH3COOH  + 
0.5          CC14 
0.2          CH3COOH  + 
0.8          CC14 
1              CC14 

58.8 
61.0 
62.4 

60.2 
57.6 

60° 

68.17 

6.735 
9,,  885 
13,98 
18.00 
22.66 
26.60 
31.66 
38.86 

54.67 
78.67 
104.6- 
128.1 
150.1 
171.9 
191.5 
210.0 

(Christoff.  J.  phys.  Ch.  1905,  53.  382.) 

CARBON  OXIDE 


173 


Absorption  of  CO2  byC2H4Cl2+CS2. 


Solvent 

cc.  CO2  absorbed 

1 
0.8 
0.2 
0.5 
0.5 
0.2 
0.8 

mol.  C2H4C12 
"   C2H4C12  + 

"  CS2 
"  C2H4C12  + 

11  CS2 
"  C2H4C12  + 

"  CS2 
"  CS2 

209.7 
173.4 
140.0 

71.9 
19.9 

(Christoff.) 


Solubility  of  CO2  in  organic  solvents 

-rr  =  change  of  solubility  for  1°  increase  in 
temp. 


Solvent 

Sol- 
ubility 
at 
25°  C. 

Sol- 
ubility 
at 
20°  C. 

Sol- 
ubility 
at 
15°  C. 

ds 
"dt 

Glycerine 

0.0302 

Water 

0.8256 

Carbon  bisulphide 

0.8699 

0^8888 

0'9446 

—0.  00747 

lodobenzene 

1.301 

.371 

1.440 

—0.0139 

Aniline 

1.324 

.434 

1.531 

—0.0207 

o-Toluidine 

1.381 

.473 

1.539 

—0.0158 

m-Toluidine 

1.436 

.581 

1.730 

—0.0244 

Eugenol 

1.539 

.653 

1.762 

—0.0223 

Benzotrichloride 

1.643 

Cumene 

1.782 

!S79 

l!978 

—  6!oi96 

Carvene 

1.802 

.921 

2.034 

—0.0232 

Dichlorhydrin 

1.810 

.917 

2.020 

—0.0210 

Amyl  alcohol 

1.831 

.941 

2.058 

—0.0227 

Brombenzene 

1.842 

.964 

2.092 

—0.0250 

Isobutyl  alcohol 

1.849 

.964 

2.088 

—  0  .  0239 

Benzyl  chloride 

1.938 

2.072 

2.180 

—0.0242 

m-Xylene 

2.090 

2.216 

2.346 

—0.0256 

Ethylene  bromide 

2.157 

2.294 

2.424 

—0.0267 

Chlorobenzene 

2.265 

2.420 

2.581 

—0.0316 

Carbon  tetrachloride 

2.294 

2.502 

2.603 

—0.0309 

Propylene  bromide 

2.301 

2.453 

2.586 

—0.0281 

Toluene 

2.305 

2.426 

2.557 

—0.0256 

Benzene 

2.425 

2.540 

2.710 

—0.0285 

Amyl  bromide 

2.455 

2.638 

2.803 

—0.0348 

Nitrobenzene 

2.456 

2.655 

2.845 

—0.0389 

Propvl  alcohol 

2  498 

Carvol 

2.498 

2.690 

2.914 

—0.0416 

Ethyl  alcohol  (97%) 

2.706 

2.923 

3.130 

—0.0424 

Benzaldehyde 

2.841 

3.057 

3.304 

—0.0463 

Amyl  chloride 

2.910 

3.127 

3.363 

—0.0453 

Isobutyl  chloride 

3.105 

3.388 

3.659 

—0.0554 

Chloroform 

3.430 

3.681 

3.956 

—0.0526 

Butyric  acid 

3.478 

3.767 

4.084 

—0.0606 

Ethylene  chloride 

3  .  525 

3.795 

4.061 

—0.0536 

Pyridine 

3.656 

3.862 

4.291 

—0.0635 

Methyl  alcohol 

3.837 

4.205 

4.606 

—0.0769 

Amyl  formate 

4.026 

4.329 

4.646 

—0.0620 

Propioriic  acid 

4.078 

4.417 

4.787 

—0.0709 

Amyl  acetate 

4.119 

4.411 

1  .  850 

—0.0731 

Glacial  acetic  acid 

4.679 

5.129 

5.614 

—0.0935 

Isobutyl  acetate 

4.691 

4.968 

—0.0554 

Acetic  anhydride 

5.206 

5.720 

6  '.218 

—0.1012 

Acetone 

6  295 

6.921 

—0.1252 

Methyl  acetate 

6.494 

(Just,  Z.  phys.  Ch.  1901.  37.  354.) 


Absorption  of  CO2  by  organic  substances-}- 
Aq  at  15°. 

P  =  %  of  the  organic  substance  in  the  sol- 
vent. 

0i 5°  =  Coefficient  of  absorption  at  15°. 

Si6°  =  Solubility  at  15°. 


Organic  substance 
used 

P 

a   ° 

P15 

S15° 

Chloral  hydrate 

0 

0.996 

0 

0.992 

l!656 

0 

1.012 

17.7 

0.885 

0.935 

21.8 

0.860 

0.908 

31.6 

0.803 

0.848 

37.0 

0.790 

G.834 

38.3 

0.781 

0.825 

49.8 

0.760 

0.802 

51.1 

0.769 

0.812 

52.6 

0.764  i     0.807 

57.1 

0.765  i     0.808 

61.1 

0.780 

0.824 

68.8 

0.797 

0.842 

71.0 

0.812 

0.857 

74.6 

0.848 

0.895 

79.4 

0.903 

0.953 

Glycerine 

0 

1.003 

1-064 

0 

1.013 

26.11 

0.785 

0.829 

27.69 

0.800 

0  845 

43  72 

0.639 

0.675 

46.59 

0.620 

0  655 

62.14 

0.511 

0.540 

73.36 

0.449 

0.474 

77.75 

0.430 

0.454 

87.74 

0.422 

0.446 

90.75 

0.404 

0.427 

96.64 

0.415 

0.438 

99.26 

0.410 

0.438 

(Hammel,  Z.  phys.  Ch.  1915,  90.  123.) 

Solubility  of  carbon  dioxide  in  solutions  of 

aniline  at  25°. 
I.  Concentration,  0.206  g.  aniline  in  100  c.  c. 

of  solution. 
P  =  Pressure. 

S  =  Solubility   calc.   according  to   formula 
given  in  original  article. 


P 

s 

p 

s 

748 
808 
920 

0.865 
0.855 
0.857 

1053 
1159 
1243 

0.855 
0.862 
0.860 

II.  Concentration,  0.425  g.  aniline  in  100  c.  c. 
of  solution. 


p 

s 

p 

s 

760 
816 
921 

0.909 
0.897 
0.897 

1150 
1236 
1380 

0.897 
0.902 
0.908 

174 


CARBON  SELENIDE 


Solubility  of  carbon  dioxide  in  solutions  of 

aniline  at  25°. — Continued 
III.  Concentration,  0.566  g.  aniline  in  100 
c.  c.  of  solution. 


p 

s 

P 

s 

760 

823 
941 

0.935 
0.929 
0.925 

1082 
1223 
1341 

0.923 
0.924 
0.930 

IV.  Concentration,   0.743  g.  aniline  in   100 
c.  c.  of  solution. 


p  1 

s 

P 

s 

760 
895 
983 

0.953 
0.941 
0.940 

1063 
1223 
1302 

0.94C 
0.940 
0.942 

(Findlay  and  Creighton,  Chem.  Soc.  1910,  97. 
555.) 

Solubility  of  CO2  in  CS2  increases  approx. 
proportionally  with  the  pressure.  The  ab- 
sorption is  preater  at  lower  temp,  and  less 
at  higher  temp,  than  is  required  by  Dalton's 
law.  (Woukoloff,  C.  R.  1889,  108.  674.) 

Absorption  of  C02  by  sugar  +Aq. 


Sugar  +Aq 

Grams  CO2  absorbed  by 
75  cc.  of  solution  at  15.5° 
and  720  mm. 

Vio-N  sugar  solution 

V-N     " 
i-N     "       " 

0.1225 
0.1089 
0.0931 

(Christoff,  Z.  phys.  Ch.  1905,  53.  329.) 
Absorption  of  C02  in  sugar +Aq  at  20°. 


Cone,  of  solution 

Sp.  gr. 

Coefficient  of 
absorption 

Vs  mol.  per  1. 

!/4  "  "  " 

v,  «  «  « 

1         a         (s    (( 

1.01518 
1.03125 
1.06372 
1.12809 

0.846 
0.815 
0.756 
0.649 

(Usher,  Chem.  Soc.  1910,  97.  72.) 

Liquid. — Not  miscible  with  H2O,  though 
slightly  sol.  therein,  or  with  fatty  oils;  mis- 
cible with  alcohol,  ether,  CS2,  and  the  essen- 
tial oils.  (Thilorier,  Mitchell.) 

Unacted  upon  by  H2O;  sol.  in  alcohol, 
ethers,  petroleum,  oil  of  turpentine,  and  CS2. 
(Mareska  and  Donny.) 

Petroleum  dissolves  5  to  6  vols.  liquid  CO2 
(Cailletet,  C.  R.  75.  1271.) 

SI.  sol.  in  CS2.    (Cailletet.) 

Solid. — When  immersed  in  H2O,  rapidly 
volatilizes  and  dissolves.  With  alcohol  or 
ether  it  forms  a  semi-fluid  mixture.  (Chan- 
ning,  Am.  J.  Sci.  (2)  5.  186.) 

Only  slightly  sol.  in  anhydrous  ether,  but 
may  be  mixed  therewith  to  a  paste.  (Thil- 
orier.) 


Sol.  in  methyl  chloride  below  — 65°  to  the 
point  of  sat.  without  decomp.  (Villard,  C.  R. 
1895,  120.  1413.) 

+6H2O.    (Villard,  C.  R.  1894,  119.  369.) 

Carbon  selenide,  C4Se. 

Sol.  only  in  hot  cone.  H2SO4.  (v.  Bartal, 
Ch.  Z.  1906,  30.  810.) 

C6Se.  Insol.  in  H2O,  CS2,  and  ether. 
Easily  sol.  in  hot  cone.  H2SO4;  sol.  in  cone. 
NaOH+Aq  from  which  it  is  pptd.  by  HC1. 
(v.  Bartal.) 

Carbon  silicide  CSi. 

(Carborundum.)  Not  attacked  by  any 
acids,  even  HF;  si.  attacked  by  caustic  al- 
kalies or  carbonates.  (Acheson,  C.  N.  68. 
179.) 

Not  attacked  by  KOH+Aq.  (Schiitzen- 
berger,  C.  R.  114.  1089.) 

Carbon  mowosulphide,  CS. 

Insol.  in  H2O,  alcohol,  oil  of  turpentine,  or 
benzene;  somewhat  sol.  in  CS2  or  ether;  sol. 
in  warm  HNOs;  sol.  in  cone.  KOH+Aq. 
(Sidot,  C.  R.  81.  32.) 

Readily  absorbed  by  alcohol  and  aniline. 
(Deninger,  J.  pr.  1895,  (2)  51.  349.) 

Carbon  ^sulphide,  CS2. 
Very  si.  sol.  in  H2O. 

1 1.  H2O  dissolves  2-3  g.  CS2  (Ckiandi,  Bull. 

Soc.  43.  562);  3.5-4.52  g,  (Peligot,  ib.  43.  563). 

30  ccm.  CS2  shaken  with  8690  com.  H2O  at 

20-23°  for  18  days  decreased  11  ccm.  in  9  days 

and  1.4  ccm.  in  the  next  3  days  by  diffused 

light,  and  0.6  ccm:  in  the  last  5  days  (no  light). 

Part  of  the  CS2  was  decomp.  and  7.85  ccm. 

were  dissolved,  therefore  H2O  dissolves  Viooo 

of  its  weight  CS2.     (Sestini,  Gazz.  eh.  it.  1. 

|  473.) 

Solubility  of  CS2  ID  H2O. 
100  pts.  H2O  dissolve  0.203  pts.  CS2  at  12-13° 
0.191       "      "    15-16° 
0.168       "      "    25-27° 
0.145       "      "     30-33°. 
(Page,  C.  N.  41.  195.) 


Solubility  of  CS2  in  H2O.    a  =  g. 
ccm.  solution  at  t°. 


CS2  in  1000 


a 

t° 

a 

t 

a 

t° 

2.04 
1.99 
1.94 

1.87 

0 
5 
10 
15 

1.79 
1.69 
1.55 
1.37 

20 
25 
30 
35 

1.11 

0.70 
0.14 

40 
45 
49 

(Chancel  and  Parmentier,  C.  R.  100.  773.) 

100  g.  H2O  dissolve  at  t°: 

t°       0  10         20         30 

0.258  0.239  0.201  0.195  g.  CS2. 

(Rex,  Z.  phys.  Ch.  1906,  55.  365.) 


CARBONATES 


175 


Absorption  of  CS2  vapor  by  H2O  at  t°. 


t° 

Coefficient 

of  absorption 

0 
10 
20 
30 

3.573 
2.189 
1.346 
0.799 

Calc.  from  data  of  Chancel  and  Parmentier, 
C.  R.  100.  733.) 

(Winkler,  Z.  phys.  Ch.  1906,  55.  352.) 

Vapors  of  C$2  are  most  easily  absorbed  by 
alcoholic  solution  of  KOH.  SI.  absorbed  by 
KOH+Aq,  and  very  slowly  by  CuS04, 
Pb(C2H3O02+Aq,  cone.  H2SO4,  or  CaCl2  in 
HCl+Aq.  (Berthelot,  A.  ch.  (3)  51.  74.) 

Solubility  in  alcohol.  S  =  strength  of  alcohol 
in  per' cent  by  weight;  P  =  pts.  CS2  which 
dissolve  in  10  ccm.  alcohol  at  17°. 


s 

p 

s 

p 

100 
98.5 
98.15 
96.95 
93.54 

oo 

18.20 
13.20 
10.00 
7.00 

91.37 
84.12 
76.02 
48.40 
47.90 

5.00 
3.00 
2.00 
0.20 
0.00 

(Tuchschmidt  and  Follenius,  B.  4.  583.) 

Miscible  with  absolute  alcohol,  ether,  ethe- 
real and  fatty  oils,  and  liquid  CO2. 

Tncarbon  bisulphide,  C3S2. 

Insol.  in  H2O;  easily  sol.  in  alcohol,  ether, 
chloroform,  benzene,  and  CS2.  The  alcoholic 
and  ethereal  solutions  decomp.  on  standing. 
(Lengyel,  B.  26.  2960.) 

Sol.  in  alcohol  with  decomp.  Sol.  in  CS2 
and  in  benzene.  (Stock,  B.  1912,  46.  3575.) 

Solid  modification.  Insol.  in  H2O  and 
ordinary  solvents.  Sol.  in  KOH+Aq. 
(Lengyel.) 

Carbon  sulphoselenide,  CSSe. 

Mpt.  — 85C,  bpt.  +84°. 

Decomp.  by  light.    Not  attacked  by  H2O. 

Sol.  in  hot  cone.  HNO3.  Decomp.  by  Br2 
to  an  oil.  Sol.  in  alcohol  with  decomp.  Mis- 
cible with  CS2.  (Stock,  B.  1914,  47.  150.) 

Carbon  sulphotelluride,  CSTe. 

Mpt,  —54°.    Very  unstable. 

Miscible  with  CS2  and  benzene  without 
decomp.  (Stock,  B.  1914,  47.  142.) 

Carbonatochloroplatindiamine     carbon- 
ate chloroplatindiamine  nitrate. 

Cl^3  [Pt  N2H6J  2(C°3)2>  Cl2Pt(N2H6N03)2. 
Precipitate.   \Cleve,  J.  B.  1867.  321.) 


Carbonatonitratoplatind'z'amine     carbon- 

ate, (  Cgs^  [Pt(N2H6)2]2(C03)2. 
Sol.  in  boiling  H2O.    (Cleve.) 

Carbonatotetramine    cobaltic    bromide, 
Co(NH3)4CO3Br. 

Much  less  sol.  than  chloride.     (Jorgensen, 
Z.  anorg.  2.  279.) 

-  carbonate,  [Co(NH3)4CO3]2CO3+3H2O. 
Very  sol.  in  H2O.    (Jorgensen.) 

-  chloraurate,    [Co(NH3)4CO3]2AuCl4  + 


Somewhat  sol.  in  H2O;  nearly  absolutely 
insol.  in  alcohol.  (Jorgensen.) 

-  chloride,  Co(NH3)4CO3Cl. 

Easily  sol.  in  H2O;  insol.  in  alcohol.  (Jor- 
gensen.) 

-  chloroplatinate,  [Co(NH3)4CO3]2PtCl6+ 
2H2O. 

Nearly  insol.  in  H2O  and  alcohol.  (Jorgen- 
sen.) 

-  chloroplatinite,  [Co(NH3)4CO3]2PtCl4. 
Nearly  insol.  in  H2O;  wholly  in  alcohol. 

(Jorgensen.) 

-  dithionate,  [Co(NH3)4CO3]2S2O6. 
Ppt.    (Jorgensen.) 

-  iodide,  Co(NH3)4CO3I. 

Much  less  sol.  than  bromide  or  chloride. 
(Jorgensen.) 

-  nitrate,  Co(NH3)4CO3NO3+^H2O. 
Sol.  in  about  15  pts.  cold  H2O;  insol.  in 

alcohol.    (Jorgensen.) 

-  sulphate,  [Co(NH3)4C03]2SO4+3H2O. 
Considerably  less  sol.  in  H2O  than  the  ni- 

trate.   (Jorgensen.) 

Carbonic  acid,  H2CO3 
See  Carbon  dioxide. 

Carbonates. 

Carbonates  of  Na,  K,  Rb,  and  Cs  are  easily 
sol.  in  H2O;  carbonates  of  Li  and  Tl  are  much 
less  sol.;  other  carbonates  are  nearly  or  quite 
insol.  All  carbonates  are  sol.  to  some  extent 
in  H2O  containing  CO2.  All  carbonates,  ex- 
cept those  of  NH4,  Rb,  and  Cs,  are  insol.  in 
alcohol. 

Sol.  in  those  acids  which  are  themselves 
sol.  in  H2O,  except  HCN  and  H3BO3. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  824.) 


176 


CARBONATE,  ALUMINUM,  BASIC 


Aluminum  carbonate,  basic. 

5A12O3,6CO2+37H2O  =  3A1(OH)3, 
A12(CO3)3  +  14H2O.       (Seubert,     Z.     anorg. 
1893,  4.  67.) 

A12O3,  CO2.  (Parkmann,  Sill.  Am.  J.  (2) 
34.  324.) 

3A12O3,  2CO2+16H2O.  (Muspratt  and 
Danson,  A.  72.  120.) 

3A12O3,  2CO2+9H2O.  (Wallace,  Chem. 
Gaz.  1868.  410.) 

5A12O3,  3CO2  +  18H2O.     (Bley,  J.  pr.  39. 

11.) 

2A12O3,  CO2+6H2O.=10A1(OH)3,  A12(CO3)3 
+3H20.  Sol.  in  cold  dil.  acids.  (Schlum- 
berger,  Bull.  Soc.  1895,  (3)  13.  46.) 

+8H2O.  (Urbain  and  Renoul.  J.  Pharm. 
(4)30.  340.)  =  10A1(OH)3,  A12(CO3)3+9H2O. 
(Seubert,  Z.  anorg.  1893.  4.  67.) 

8A12O3,  3CO2+40H2O.  (Langlois,  A.  ch. 
(3)  48.  505.) 

All  are  precipitates,  insol.  in  H2O,  sol.  in 
acids,  and  give  off  CO2  at  slight  heat. 

There  are  no  definite  carbonates  of  alum- 
inum. (Cameron,  J.  phys.  Chem.  1908,  12. 
572.) 

Aluminum  ammonium  carbonate,  A12O3,  CO2, 

(NH4)2CO3+4H20. 
Precipitate.    (Rose,  Pogg.  91.  460.) 

Aluminum   sodium    carbonate,   A12O3,    CO2, 

2Na2CO3+24H2O. 

Precipitate.  Sol.  in  cold  dil.  acids.  (Bley, 
J.  pr.  39.  22.) 

Ammonium  carbonate,  (NH4)2C03+H2O. 

Sol.  at  15°  in  its  own  weight  H2O.  Solution 
in  H2O  gives  off  gas  at  70-75°,  and  boils  at 
75-80°.  SI.  sol.  in  cold  dil.  NH4OH+Aq, 
more  sol.  at  ordinary  temp.  Insol.  in  cone. 
NH4OH+Aq.  (Divers,  Chem.  Soc.  (2)  8. 
171,  259,  and  364.)  .  . 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  826.) 

Insol.  in  alcohol. 

Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.257.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

100  g.  pure  glycerine  dissolve  20  g. 
(NH4)2CO3  at  15°.  (Ossendowski,  Pharm.  J. 
1907,  79.  575.) 

Ammonium  hydrogen  carbonate,  NH4HCO3. 

Sol.  at  15°  in  about  8  pts.  H2O.  (Berthol- 
let,  J.  Phys.  66.  168.) 

Sol.  at  12.8°  in  about  6  pts.  H2O.  (J.  Davy, 
N.  Edinb.  J.  16.  245.) 

Solution  decomp.  on  air  or  by  gentle  heat  or 
by  addition  of  the  solid  salt.  (Berthollet.) 

100  pts.  H2O  dissolve  at  0°,  11.9  pts.;  at 
10°,  15.85  pts.;  at  20°,  21  pts.;  at  30°,  27  pts. 
NH4HCO3.  (Dibbits,  J.  pr.  (2)  10.  417.) 


Solubility  of  NH4HCO3  in  NH4Cl+Aq,  sat 
with  CO2,  at  t°. 


t° 

g.  per  10 

0  g.  H20 

Sp.  gr.  of  sat. 

NH4C1 

NH4HCO3 

solution 

0° 

0 
29.08 

11.9- 
3.6 

T077 

15° 

0 
2.99 
6.06 
8.51 
11.68 
18.30 
26.93 
33.25 
34.35 

18.64 
16.29 
14.22 
12.69 
11.68 
9.33 
7.73 
6.64 
6.42 

1.064 
.063 
.062 
.062 
.065 
.069 
.076 
.085 
.085 

30° 

0 
39.7 

27.0 
9.1 

(Fedotieff,  Z.  phys.  Ch.  1904,  49.  168.) 

Solubility   of   NH4HCO3   in   NaHCO3+Aq, 
sat.  with  CO2  at  t°. 


t° 

g.  per  100  g.  H2O 

Sp.  gr.  of  sat. 
solution 

XaHCOs 

NH.HCOs 

0° 
15° 

0 

4.82 

11.90 
10.94 

1.072 

0 
5.92 

18.64 
17.06 

1.064 
1.090 

30° 

0 
7.0 

27.0 
23.0 

(Fedotieff,  Z.  phys.  Ch.  1904,  49.  168.) 
Solubility  of  NH4HCO  3  in  NH4NO3  -f  Aq  at  t°. 

t° 

g.  per  100  g.  H2O 

Sp.  gr.  of  sat. 
solution 

NH4NO3 

NH4HCO 

0° 

0 
118 

11.90 
4.52 

1^2625 

15° 

0 
23.26 
49.82 
103.4 
128.9 
166.9 

18.64 
12.91 
10.33 
8.25 
7.79 
7.49 

1.064 
1.113 
1.164 
1.242 
1  .  269 
1.302 

30° 

0 
231.9 

26.96 
12.57 

(Fedotieff  and  Koltunoff,  Z.  anorg.  1914,  85. 
251.) 

Insol.  in  alcohol.    (J.  Davy.) 
Insol.  in  acetone.     (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 


CARBONATE,  AMMONIUM  DYSPROSIUM 


177 


Ammonium  dihydrogen  carbonate, 

(NH4)4H2(C03)3+H20. 

Sp.   gr.   of  carbonate   of  ammonia  +Aq   at 
12°.—  Continued 

Sol.  in  5  pts.  H2O  at  15°;  decomp.  by  more 
H2O  or  by  heat.     (Divers,  Chem.  Soc.  (2)  8. 
171,  359,  and  364.) 

Deg.  Tw. 

Spjr.  at 

%  Carb. 
arnmon. 

Change  of 
sp.  gr. 

£           1  O    /"I 

SI.  sol.  in  alcohol. 

for  1°  C. 

18 

1.090 

26.82 

0.0007 

Ammonium  hydrogen  carbonate   carbamate, 

19 

1.095 

28.33 

0.0007 

2NH4HC03,  NH4CONH2.    (Salts  of  harts- 

20 

1.100 

29.93 

0.0007 

horn.) 

21 

1.105 

31.77 

0.0007 

1  pt.  salt  dissolves  at: 

22 

1.110 

33.45 

0.0007 

13°     in  4     pts.  H2O. 

23 

1.115 

35.08 

0.0007 

16.7°   "3.3 

24 

1.120 

36.88 

0.0007 

32.2°   "  2.7        " 

25 

1.125 

38.71 

0  0007 

40.6°   "2.4        " 

26  ' 

1  .  130 

40.34 

0.0007 

49°      "  2           " 

27  . 

1.135 

42.20 

0.0007 

(J.  Davy,  N.  Edinb.  J.  16.  245.) 

28 
29 

1.140 
1.144 

44.29 
44.90 

0.0007 
0.0007 

Strong  alcohol  dissolves  out  carbamate,  and 
the  carbonate  remains  undissolved. 

NH4HC03,  NH4C02NH2.  (Commercial 
carbonate  of  ammonia.) 

Sol.  at  15°  in  4  pts.  H2O,  at  65°  in  \Y2  pts. 
H20.  (Divers.) 

30  pts.  salt +100  pts.  H2O  lower  temp,  from 
15.3°  to  3.2°.  (Rudorif,  B.  2.  68.) 

So!,  in  1.667  pts.  cold,  and  0.833  pt.  hot  H2O.  (Four- 
croy.) 

100  pts.  H2O  at  13°  dissolve  25  pts. 
17°  "  30  " 
37°  "  37  " 
41°  "  40  " 
49°  50  " 

(Berzelius.) 

100  pts.  H2O  at  15.5°  dissolve  33  pts.;  at  100°,  100 
pts.  (lire's  Diet.) 

89!.  in  2  pts.  H2O  at  15.5°,  and  in  less  than  1  pt. 
boiling  H2O;  sat.  solution  at  15.5°  contains  33.3%,  and 
sat.  boiling  solution  50%.  (Abl.) 

Sat.  aqueous  solution  at  10°  contains  15.7%.    (Eller.) 
Sat.  aqueous  solution  at  (?)  contains  6.1%.    (Mus- 
sembroek.) 

Sat.  solution  in  the  cold  contains  37.5%.    (Fourcroy.) 
Does  not  dissolve  as  such  in  H2O;  (NH^izCOs  dis- 
solves out  first,  and  NH4HCO3  later.     (Scanlan.) 

Sp.  gr.  of  carbonate  of  ammonia+Aq  at  12°. 


Deg.  Tw. 

Sp.  gr.  at 
12°. 

%  Carb. 

.•minion. 

Change  of 
sp.  gr. 
for  1°  C. 

1 

1.005 

1.66 

0.0002 

2 

1.010 

3.18 

0.0002 

3 

1.015 

4.66 

0.0003 

4 

1.020 

6.04 

0.0003 

5 

1.025 

7.49 

0.0003 

6 

.  1.030 

8.93 

0.0004 

7 

1.035 

10.35 

0.0004 

8 

1.040 

11.86 

0.0004 

9 

1.045 

13.36 

0.0005 

10 

.050 

14.83 

0.0005 

11 

.055 

16.16 

0.0005 

12 

.060 

17.70 

0.0005 

13 

.065 

19.18 

0.0005 

14 

.070 

20.70 

0.0005 

15 

.075 

22.25 

0.0006 

16 

.080 

23.78 

0.0006 

17 

1.085 

25.31 

0.0006 

(Lunge,  Chem.  Ind.  1883.  2.) 

Sp.  gr.  of  aqueous  solution  of  salt  with  com- 
position 31.3%  NH3,  56.6%  CO2,  12.1% 
H2O.     100  pts.  of  solution  contain — 
6.58      9.96      14.75    19.83    25.71  pts.  salt 

1.0219  1.0337  1.0497  1.0672  1.0863  sp.  gr. 

29.74      35.85      40.23      44.90  pts.  salt. 
1.0995     1.1174     1.1297     1.1414  sp.  gr. 
(J.  H.  Smith,  Chem.  Ind.  1883.  3.) 

Cone,  alcohol  dissolves  out  carbamate  and 
leaves  carbonate.    (Hiinefeld,  J.  pr.  7.  25.) 
Insol.  in  acetone.    (Naumann,  B.  1904,  37. 

4328.) 

Ammonium    cerous   carbonate,    (NH4)2CO3, 

Ce2(CO3)3+6H2O. 

Ppt.  Very  si.  sol.  in  cone.  (NH4)2CO3+Aq. 
(Meyer,  Z.  anorg.  1904,  41.  104.) 

Ammonium  chromous  carbonate,  (NH4)2CO3t 

CrCO3+H2O. 

Decomp.  by  moist  air;  sol.  in  dil.  HC1  and 
H2SO4.  (Bauge",  C.  R.  1896,  122.  476.) 

Ammonium  cobaltous  carbonate,  (NH4)2CO3, 
CoCO3+4H2O. 

Permanent.  Sol.  in  H2O.  (Deville,  A.  ch. 
(3)  36.  460.) 

(NH4)2O,  2CoO,  4C02+9H2O.  Quickly  de- 
comp. on  air:  sol.  in  H2O.  (Deville.) 

+12H2O.    Sol.  in  H2O. 

Ammonium  didymium  carbonate,  (NH4)2COS, 

Di2(C03)3+3H20. 
Insol.  in  H2O.    (Cleve.) 

Ammonium  dysprosium  carbonate, 

NH4Dy(C03)3+H20. 
Only  si.  sol.  in  H2O.    (Jantsch,  B.  1911,  44. 

1277.) 


178 


CARBONATE,  AMMONIUM  GLUCINUM 


Ammonium  glucinum  carbonate,  2(NH4)2CO3, 
3G1CO3(?). 

Very  sol.  in  cold,  decomp.  by  hot  H2O. 
Nearly  insol.  in  alcohol.  (Debray.) 

Composition  is  (NH4)2CO3,  2G1CO3, 
G1(OH)2+2H2O.      (Humpidge,    Royal    Soc. 
Proc.  39.  1.) 

Ammonium  lanthanum  carbonate,  La2(CO3)3, 

(NH4)2C03+4H20. 
Ppt.    (Meyer,  Z.  anorg.  1904,  41.  102.) 

Ammonium  magnesium  carbonate, 

(NH4)2Mg(C03)2+4H20. 

Sol.  in  71  pts.  H2O  with  decomp.;  more 
sol.  in  NH4Cl-f  Aq.  (Divers,  Chem.  Soc.  51. 
196.) 

H2O  containing  (NH4)2CO3  dissolves  very 
slightly;  more  sol.  in  H2O  containing  NH4C1. 
(Favre,  A.  ch.  (3)  10.  473.) 

Ammonium  magnesium  hydrogen  carbonate, 

(NH4)2Mg2H2(CO3)4+8H2O,  or  12H2O. 
Decomp.  on  air.     (Deville,  A.  ch.  (3)  35. 
454.) 

Ammonium  neodymium  carbonate, 
(NH4)2CO3,  Nd2(C03)3+4H2O. 
Ppt.     SI.    sol.   in   cone.    (NH4)2CO3+Aq. 
(Meyer,  Z.  anorg.  1904,  41.  106.) 

Ammonium    nickel    carbonate,    NH4HCO3, 

NiCO3-t-4H2O. 
Insol.  in  H2O.    (Deville,  A.  ch.'(3)  35.  452.) 

Ammonium  praseodymium  carbonate, 

(NH4)2C03,  Pr2(C03)3+4H20. 
Ppt.     Insol.  in  (NH4)2CO3+Aq.     (Meyer, 
Z.  anorg.  1904,  41.  105.) 

Ammonium  samarium  carbonate,  (NH4)2C03, 

Sm2(CO3)3+4H2O. 
Ppt. 

Ammonium  scandium  carbonate,  (NH4)2CO3, 

.    2Sc2(C03)3+6H20. 

Difficultly  sol.  in  H2O.  Sol.  in  cold  alkali- 
carbonate  4-Aq,  less  sol.  in  hot.  (R.  Meyer, 
Z.  anorg.  1910,  67.  410.) 

Ammonium  tin  (stannous)  carbonate, 

(NH4)2CO3,  2SnCO3+3H2O. 
Decomp.  by  cold  H2O.    (Deville,  A.  ch.  (3) 

Ammonium  uranyl  carbonate,  2(NH4)2CO3, 
U02CO3. 

Sol.  at  15°  in  20  pts.  H2O,  more  abundantly 
in  H2O  containing  (NH4)2CO3.  (Ebelmen.) 

Insol.  in  pure  H2O;  sol.  in  H2O  containing 
(NH4)2CO3.  Solution  is  decomp.  by  boiling. 
(Berzelius.) 


Sol.  in  SO2+Aq.  (Berthier,  A.  ch.  (3)  7. 
76.) 

3(NH4)2CO3,  2(UO2)CO3+4H2O.  Sol.  in 
H2O.  (Giolitti  C.  C.  1905,  II.  227.) 

Ammonium  vanadyl  carbonate,  3(NH4)2O, 
7VO2,  5CO2+16H2O. 

SI.  sol.  in  H2O. 

Sol.  in  acids  and  alkalies.  •  (Koppel,  Z. 
anorg.  1905,  45.  350.) 

Ammonium  yttrium  carbonate,   (NH4)2GO3, 

Y2(C03)3+2H20. 
Insol.  in  (NH4)2CO3+Aq.     (Mosander.) 

Ammonium    zinc    carbonate,    basic,    3ZnO, 

NH4OH,  2CO2+H2O. 
Insol.  in  H2O.    (Kassner,  Arch.  Pharm.  (3) 
27.  673.) 

Ammonium  zinc  carbonate,  (NH4)2CO3, 
ZnCO3. 

Insol.  in  H2O.    (Deville.) 

Quite  sol.  in  H2O;  more  sol.  than 
(NH4)2CO3,  MgCO3.  Tolerably  permanent 
in  the  air.  Slowly  decomp.  by  cold,  rapidly 
by  hot  H2O. 

Very  sol.  in  (NH4)2CO3+Aq.  Not  attacked 
by  alcohol.  (Favre,  A.  ch.  (3)  10.  481.) 

Barium  carbonate,  BaCO3. 

Sol.  in  4304  pts.  cold,  and  2304  pts.  boiling 
H2O.  (Fourcroy.) 

Sol.  in  47,620  pts.  H2O.  (Bineau,  A.  ch. 
(3)  51.  290.) 

Sol.  in  14,137  pts.  H2O  at  16-20°,  and 
15,421  pts.  at  100°.  (Fresenius.) 

Sol.  in  12,027  pts.  H2O  at  15°.  (Kremers, 
Pogg.  85.  247.) 

Calculated  from  electrical  conductivity  of 
solution,  1  pt.  BaCOs  is  sol.  in  64,070  pts.  H2O 
at  8.8°  and  45,566  pts.  at  24.2°.  (Hollemann, 
Z.  phys.  Ch.  12.  125.) 

Solubility  in  H2O  at  t°. 


14 
18 
23 
27 
32 
38 


g.  sol.  in  100  g.  H2O 


4.32  x  10-4 
4.57  x  10-4 
4.89  x  10-4 
5.22  x  10-4 
5.69  x  1C-4 
6.27  x  10-4 


(Weissenberger,  Z.  phys.  Ch.  1914,  88.  266.) 

"Solubility  product"  =8.1  x  10-'  mol.  1. 
(McCoy  and  Smith,  J.  Am.  Chem.  Soc.  1911, 
33.  473.) 

Sol.  in  H2CO3+Aq.  (See  barium  hydrogen 
carbonate.} 

Easily  sol.  in  dil.  acids.  Not  acted  upon  by 
cone.  HNO3+Aq. 

Not  decomp.  by  1  pt.  H2SO4+6  pts.  ab- 
solute alcohol.  Slowly  decomp.  by  1  pt. 


CARBONATE,  BARIUM  URANYL 


179 


HNO3+6  pts.  absolute  alcohol.  Slowly  de- 
comp.  by  1  pt.  H2G2O4+6  pts.  absolute  al- 
cohol. 

Not  decomp.  by  absolute  alcoholic  solu- 
tions of  racemic,  tartaric,  citric,  or  glacial 
acetic  acids.  (Babington  and  Phillips,  1816.) 

Almost  completely  insol.  in  H2O  containing 
NH4OH  and  (NH4)2CO3,  when  digested  in 
such  a  solution  and  allowed  to  stand.  1  pt. 
BaCO3  dissolves  in  141,000  pts.  of  such  a  solu- 
tion. (Fresenius.) 

Not  more  sol.  in  NaCl+Aq  than  in  H2O. 
(Karsten.) 

Sol.  in  cold  NH4C1,  NH4NO3,  or  NH4  suc- 
cinate+Aq.  (Vogel,  J.  pr.  7.  453.) 

2  mols.  NH4C1  dissolved  in  H2O  dissolve  1 
mol.  BaCO3  by  continued  boiling.  (Smith, 
Phil.  Mag.  J.  9.  540.) 

Solubility  in  H2O  increases  by  addition  of 
NH4C1,  at  first  strongly,  then  less  strongly 
and  finally  strongly  again.  (D'Agustino  and 
Pellegrino,  Gazz.  ch.  it.  1908,  38  (1)  532.) 

Somewhat  sol.  in  K2CO3+Aq.  (Wacken- 
roder,  A.  24.  30.) 


Solubility  of  BaCO3  in  KCl+Aq  at  bpt.  of 
solution 


g.  KC1  per  100  g. 
solution 

g.  BaCOs  per  1000  cc.  sat. 
solution 

0.15 

0.0847 

1 

0.1781 

3 

0.2667 

10 

0.4274 

30 

0.5550 

(Cantoni  and  Goguelia,  Bull.  Soc.  1905,  (3) 
33.  13.) 


Solubility  of  BaCO3  in  NaCl+Aq  at  bpt.  of 
solution 


g.  NaCl  per  100  g. 
solution 

g.  BaCOs  per  1000  cc 
solution 

sat. 

0.15 

0.0587 

1 

0.0787 

3 

0.1056 

10 

0.1575 

30 

0.2784 

(Cantoni  and  Goguelia,  1.  c.) 
Solubility  of  BaCO3  in  10%  KCl+Aq  at  t°. 


t° 

g.  BaCOs  per  1000  cc.  sat. 
solution 

10 
20 
40 
60 

80 

0.2175 
0.2408 
0.2972 
0.3491 
0.4049 

(Cantoni  and  Goguelia,  1.  c.) 


Solubility  of  BaCO3  in  10%  NaCl+Aq  at  tc 


t° 

g.  BaCOa  per  1000  cc.  sat. 
solution 

10 
20 
40 
60 

80 

0.1085 
0.1126 
0.1231 
0.1303 
0.1418 

(Cantoni  and  Goguelia,  1.  c.)  • 

Slowly  sol.  in  cone.  Na2SO4,  MgSO4,  ZnSO4, 
Ca(NO3)2,  or  CaCl2+Aq,  but  insol.  in  ZnCl2 
-f-Aq.  (Karsten.) 

SI.  decomp.  by  boiling  K2SO4+Aq. 

SI.  decomp.  in  the  cold  by  1  pt.  K2SO4+2 
pts.  Na2SO4+Aq. 

'Decomp.  by  salts  of  Al,  Mn,  Cr,  Fe,  U,  Bi, 
Cd,  Cu,  Hg,  Pb,  Sn",  Sniv,  Hg2,  Rh,  Ir,  Au, 
with  pptn.  of  oxide  of  metal.  (Rose,  Tr.) 

Pptn.  of  BaCO3  is  hindered  by.  presence  of 
alkali  citrates  or  metaphosphates. 

Sol.  in  solutions  of  various  salts,  as  in  the 
case  of  calcium  carbonate  (see  Calcium  car- 
bonate) .  The  solvent  power  of  these  solutions 
for  barium  carbonate  is  somewhat  less  than 
for  calcium  carbonate. 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
B.  1909,  42.  3790) ;  ethyl  acetate.  (Naumann, 
B.  1904,  37.  3602.) 

Insol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

Min.  Witherite. 

Barium  hydrogen  carbonate,  BaH2(CO3)2(?). 

100  pts.  H2O  containing  CO2  dissolve  0.079 
pt.  BaCO3.  (Bineau.) 

100  pts.  H2O  containing  CO2  dissolve  0.17 
pt.  BaCO3.  (Lassaigne.) 

100  pts.  H2O  sat.  with  CO2  under  a  pressure 
of  4-6  atmospheres  dissolve  0.725  pt.  BaCO3. 
Upon  evaporating,  BaCO3  is  deposited. 
(Wagner,  Z.  anal.  6.  167.) 

BaCO3  is  sol.  in  833  pts.  H2O  sat.  with  CO2 
at  10°.  (Lassaigne.) 

BaCO3  is  sol.  in  830  pts.  H2O  sat.  with  CO2 
at  10°.  (Fourcroy.) 

BaCO3  is  sol.  in  1550  pts.  H2O  sat.  with  CO2 
at  10°.  (Bergman.) 

100  cc.  H2O  sat.  with  CO2  dissolve  0.73  g. 
BaH2(CO3)2.  (McCoy  and  Smith,  J.  Am. 
Chem.  Soc.  1911,  33.  473.) 

Barium  calcium  carbonate,  BaCO3,  CaCO3. 

Min.  Barytocalcite,  Bromlite.  Sol.  in  dil. 
acids. 

Barium  uranyl  carbonate,  BaO,  2UO3,  2CO2 
+5H-.O.  Decomp.  by  H2O.  (Blinkoff. 
Dissert.  1900.) 

+8H2O.    Decomp.  by  H2O.    (Blinkoff.) 


180 


CARBONATE  BISMUTH,  BASIC 


Bismuth   carbonate,   basic,    (BiO)2CO3  + 


Insol.  in  H2O;  sol.  in  acids.  Insol.  in  CO2  + 
Aq.  (Bergman.) 

Completely  sol.  in  (NH4)2CO3+Aq;  si.  sol. 
in  K2CO3+Aq.;  insol.  in  Na2CO3+Aq.  (Lau- 
gier.) 

Absolutely  insol.  in  (NH4)2CO3+Aq  unless 
H3PO4  or  H3AsO4  are  present.  (Berzelius.) 

Insol.  in  (NH4)2CO3,  K2CO3,  or  Na2CO3  + 
Aq.  (Rose.) 

Sol.  in  NH4Cl+Aq.  (Wackenroder.)  In- 
sol. in  NH4NO3+Aq.  (Brett.) 

Sol.  in  CaCl2+Aq.    (Pearson.) 

Min.  Bismuthosphaerite. 

3Bi2O3,  CO2.  Min.  Bismuthite.  Easily 
sol.  in  acids. 

4Bi2O3,  3CO2+4^H2O.  Min.  Bismuth 
spar.  Easily  sol.  in  acids. 

Bismuth  potassium  carbonate,  Bi2OK4(CO3)4 

+H20.. 

Decomp.  by  large  quantities  of  H2O.  (Rey- 
nolds, Chem.  Soc.  1898,  73.  266.) 

Cadmium  carbonate,  CdC03. 

Insol.  in  H2O;  easily  sol.  in  acids;  insol.  in 
K2CO3,  and  Na2C03+Aq;  very  si.  sol.  in 
(NH4)2CO3+Aq.  (Fresenius.) 

Easily  sol.  in  NH4  sulphate,  nitrate,  and 
succinate+Aq.  (Wittstein.) 

Sol.  in  KCN+Aq;  sol.  in  cold  NH4Cl+Aq; 
less  sol.  in  NH4NO3+Aq.  (Brett,  1837.) 

Not  prevented  from  pptn.  by  non-  volatile 
organic  substances.  (Rose.) 

Not  pptd.  from  solutions  containing  sodium 
citrate.  (Spiller.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,20.827.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790)  ;  'ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

+  3^H2O.    (Lefort,  J.  B.  1847.  346.) 
(Kraut,  Z.  anorg.  1897,  13.  14.) 

Cadmium  carbonate  hydrazine,   CdCO3, 

2N2H4. 

Easily  sol.  in  cold  NH4OH  +  Aq.  (Franzen, 
Z.  anorg.  1908,  60.  281.) 

Caesium  carbonate,  Cs2CO3. 

Very  deliquescent,  and  sol.  in  H2O. 

100  pts.  absolute  alcohol  dissolve  11.1  pts. 
Cs2CO3  at  19°;  20.1  pts.  Cs2CO3  at  boiling 
temp.  (Bunsen.) 

Caesium  hydrogen  carbonate,  CsHCO3. 
Not  deliquescent.    Sol.  in  H2O. 

Calcium  carbonate  basic,  CaO,  CaCO3+H2O. 
Hardened    by    H2O,    but    not    dissolved. 
(Raoult,  C.  R.  92.  189.) 


Calcium  carbonate,  CaCO3. 

More  sol.  in  cold  than  in  hot  H2O.     (Gmeliii.) 
When  recently  pptd.,  sol.  in  8834  pts.  boiling,  and 
10,601  pts.  cold  EhO;  much  less  sol.  in  H2O  containing 
NH4OH  and  (NH^COs,  65,246  pts.  of  which  dissolve 
1  pt.  CaCOs.     (Fresenius  (1846),  A.  59.  122.) 
Sol.  in  16,000  pts.  pure  H2O.     (Brandes,  1825.) 
Sol.  in  12,858  pts.  pure  H2O  at  15°.    (Kremers,  Pogg. 

Sol.  in  16,000-24,000  pts.  pure  H2O.     (Bucholz.) 

1  1.  H2O  dissolves  34  mg.  CaCO3.  (Cheva- 
let,  Z.  anal.  8.  91;  Hoffmann,  Z.  anal.  4.  414.) 

1  1.  H2O  may  contain  0.016  g.  CaCO3.  i.  e., 
1  pt.  is  sol.  in  62.500  pts.  H2O.  (Bineau,  A. 
ch.  (3)  51.  290.) 

1  1.  H2O  dissolves  0.02  g.  CaC03,  i.  e.,  1  pt. 
CaCO3  is  sol.  in  50.000  pts.  H2O.  (Peligot.) 
Solubility  is  much  affected  by  CO2  of  the  air. 

1  1.  H2O  at  16°  dissolves  13.1  mg.  CaCO3. 
(Schlcsing,  C.  R.  74.  1552.) 

Calculated  from  electrical  conductivity  of 
CaCO3+Aq,  1  pt.  CaCO3  is  sol.  in  99,500  pts. 
H2O  at  8.7°,  and  80,040  pts.  at  23.8°.  (Holle- 
mann,  Z.  phys.  Ch.  12.  125.) 

By  continued  boiling  CaH2(CO3)2,  36  mg. 
CaCO3  remain  in  solution.  (Weltzien,  A.  136. 
165.) 

Solubility  in  H2O  at  different  pressures. 


Pressure  in  atmos. 


Solubility 


1079 
1403 
1820 
2109 


(Engel,  C.  R.  101.  949.) 

100  pts.  H2O  dissolve  C.0005  pt.  (calculated 
as  CaO)  from  pptd.  CaCO3,  and  0.0027  pt. 
from  calcspar.  (Lubavin,  J.  russ.  Soc.  24. 
389.) 

1  1.  H2O  dissolves  13  mg.  CaCO3  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1893,  12.  241.) 

1  1.  CO2  free  water  dissolves  17.4  mg.  CaO 
or  31.0  mg.  CaCO3.  (Gothe,  Ch.  Z.  1915, 
39.  305.) 

CaCO3  dissolves  in  9662  pts.  H2O  at  12°. 
(Pollacci,  C.  C.  1896,  II.  946.) 

1  1.  H2O  free  from  CO2  dissolves  9.6  mg. 
CaCO3.  (McCoy  and  Smith,  J.  Am.  Chem. 
Soc.  1911,  33.  473.) 

Found  dissolved  in  10,000  pts.  sea  water. 
(Davy.) 

Pptd.  amorphous  CaCO3  dissolves  in  1600 
pts.  sea  water.  Pptd.  crystalline  CaCO3  dis- 
solves in  8000  pts.  sea  water.  (Irvine  and 
Young,  Chem.  Soc.  66.  344.) 

Artificial  sea  water  sat.  with  CO2  dissolves 
CaCO3  corresponding  to  57.27  mg.  of  com- 
bined CO 2  per  litre  at  15°. 

Sea  water  which  contains  52-55  mg.  neutral 
combined  CO2  per  litre  must  be  sat.  with 
CaCO3.  (Cohen,  Chem.  Soc.  1900,  78  (2) 
725.) 

For  action  of  H2CO3+Aq,  see  Calcium 
hydrogen  carbonate. 


CARBONATE,  CALCIUM 


181 


Sol.  in  H2SO4,  eyen  when  native.  Sol.  in 
acids  generally.  When  treated  with  acids  in 
closed  vessels  effervescence  ceases  on  increase 
of  pressure,  but  is  renewed  at  once  on  remov- 
ing it.  (Link,  1814.) 

Unacted  upon  by  cone.  HNO3,  even  when 
boiling,  as  Ca(N03)2  is  insol.  in  cone.  HNO3. 

Not  decomp.  by  mixture  of  1  pt.  H2SO<,  and 
6  pts.  absolute  alcohol,  but  immediately  by 
HNO 3+ absolute  alcohol. 

Not  decomp.  by  absolute  alcoholic  solutions 
of  oxalic,  racemic,  tartaric,  citric,  or  glacial 
acetic  acids.  (Babington  and  Phillips,  1816.) 

Unacted  upon  by  glacial  HC2H3O2,  even 
when  boiling. 

Freshly  pptd.  CaCO3  is  sol.  in  cold  NH4C1+ 
Aq ;  but  the  solution  becomes  'cloudy  on  ex- 
posure to  air,  a  portion,  however,  of  CaC03 
remains  dissolved,  which  cannot  be  pptd.  even 
by  boiling.  If  ppt.  is  washed  and  allowed  to 
stand  24  hours,  it  is  not  as  sol.  in  NH4C1  as 
at  first,  but  natural  CaCO3  is  not  wholly 
insol.  in  NH4Cl+Aq;  it  is,  however,  much 
less  sol.  than  MgCO3.  (Vogel,  J.  pr.  7.  453.) 

Sol.  in  boiling  NH4Cl+Aq  with  evolution 
of  NH3.  (Demarcay,  1834.) 

When  TSlH4OH+Aq,  incompletely  sat.  with 
CO2,  is  mixed  with  CaCl2+Aq,  no  ppt.  occurs 
even  during  several  days,  if  kept  in  a  closed 
vessel;  and  only  a  slight  ppt.  if  the  mixture 
is  exposed  to  the  air,  but  CaCO3  is  pptd.  if 
the  solution  is  boiled. 

NH4OH+Aq  wholly  sat.  with  CO2  pro- 
duces ppt.  when  mixed  with  OaCl2+Aq,  but 
pptn.  is  not  complete  until  heat  is  applied. 
Also  when  an  excess  of  CaCl2+Aq  is  added  to 
a  solution  of  crystallized  carbonate  of  am- 
monia, orly  a  portion  of  the  CaCO3  is  pptd. 
until  the  solution  is  boiled.  (Vogel,  1814.) 

When  CaCl2+Aq  mixed  with  NH4OH+Aq 
is  exposed  to  an  atmos.  of  pure  CO2,  no  ppt. 
occurs  for  several  hours,  but  CaCO3  is  com- 
pletely pptd.  in  several  days.  (Vogel.) 

When  recently  pptd.,  readily  sol.  in  NH4C1, 
and  NH4NO3+Aq.  (Brett,  1837;  Wacken- 
roder,  A.  41.  315.) 

When  recently  pptd.,  readily  sol.  in 
(NH4)2C03,  (NH4)2SO4,  NH4NO3,  NH4C1, 
and  NH4  succinate+Aq.  (Wittstein.) 

Sol.  in  NH4C2H3O2+Aq.    (Thomson.) 

More  sol.  in  NH4C1,  or  NH4N03+Aq,  or 
in  neutral  potassium,  or  sodium  salts -j-Aq 
than  in  H2O.  (Fresenius.) 

From  solutions  in  NH4  salts,  NH4OH,  and 
(NH4)2CO3+Aq  precipitate  CaCO3  more 
completely  than  BaCO3.  (Fresenius.) 

When  boiled  with  NH4Cl+Aq,  CaCO3  is 
dissolved,  and  (NH4)2CO3  given  off.  (D. 
Smith.) 

CaCl2+Aq  prevents  pptn.  of  CaCO3  in  the 
cold,  as  do  also  NH4C1,  KC1,  or  NaCl+Aq, 
but  it  is  pptd.  when  boiled,  if  the  latter  solu- 
tions are  not  too  cone.  K2SO<,  KNO3, 
(NH,)2SO,,  or  Na2SO4+Aq  have  a  similar 
effect.  A  large  excess  of  (NH^COs+Aq 
when  quickly  added  to  CaCl2+Aq  produces 


no  ppt.  in  the  cold.  Na2CO3,  or  K2CO3+Aq 
act  likewise.  (Storer,  Am.  J.  Sci.  (2)  26.  41.) 

1  g.  CaCO3  requires  13.98  g.  NH4C1,  8.380 
g.  (NH4)2SO4,  or  14.438  g.  NH4NO3  to  effect 
solution.  (Bertrand,  Monit.  Sci.  (3)  10.  477.) 

Less  sol.  in  Na  than  in  NH4  salts,  but  more 
than  in  K  salts.  (Berthelot.) 

When  NH4OH+Aq,  partially  neutralized 
by  CO2,  is  mixed  with  CaO2H2+Aq,  no 
cloudiness  appears  until  the  mixture  is  boiled; 
when  more  CO2  has  been  added  to  NH4OH  + 
Aq,  a  ppt.  appears  at  first,  which  disappears 
and  only  reappears  on  addition  of  much 
CaO2H2+Aq;  but  NH4OH+Aq  does  not 
dissolve  pptd.  CaC03.  (Vogel.) 

Solubility  in  NH4  salts +Aq  at  25°. 


NH4  salt 

Millimols 
NH4  salt 
per  1. 

Millimols 
CaO  dis- 
solved per  1. 

NH4C1 

1000 
500 

250 
125 

6.770 
5.008 
3.724 
2.743 

NH4NO3 

500 
250 
125 
62.5 

5.267 
3.830 
2.779 
2.004 

Triammonium  citrate 

500 
250 
125 
62.5 

66.87 
39.80 
22.64 
14.92 

(Rindell,  Z.  phys.  Ch.  1909,  70.  454.) 


Solubility  of  CaCO3  in  NH4Cl+Aq  at  12-18°. 
Time,  98  days. 


g.  per  1.  of  sat.  solution 

NH«C1 

CaCOa 

53.5 
100 

200 

0.423 
0.609 
0.645 

(Cantoni  and  Goguelia,  Bull.  Soc.  1905,  (3) 
33.  27.) 

Solubility  of  CaCO3  in  NH4NO3+Aq  at  18°. 


g.  per  1.  of  sat.  solution 

NHiNOs 

CaCOs 

0 
5 
10 

20 
40 
80 

0.131 
0.211 
0.258 
0.340 
0.462 
0.584 

(Berju 

and   Kosminiko,    Landw.   Vers.   Sta. 
1904,  60.  422.) 

182 


CARBONATE,  CALCIUM 


CaO2H2+Aq    dissolves    a    little    CaCO; 
(Welter  and  Berthollet,  1789.) 

CaO2H2+Aq  retains  a  little  CaCO3  in  solu- 
tion at  ordinary  temperature,  which  is  pptd. 
on  boiling.  (Eliot  and  Storer.  Proc.  Am.  Acad. 
1860.  5.  63.) 

CaO2H2+Aq,  mixed  with  dil.  NaOH,  KOH, 
or  NH4OH+Aq,  gives  no  immediate  ppt. 
when  CO2  is  passed  through  it,  unless  boiled. 

Sol.  in  boiling  MgCl2+Aq  even  when  dilute. 
Couste".) 

Not  decomp.  when  boiled  with  K2SO4, 
Na2SO4,  CaS04,  MgSO4,  and  Na2B4O:+Aq; 
but  partially  decomp.  by  boiling  with 
(NH4)2S04,  K2S03,  Na2S03,  (NH4)2SO3, 
Na2HPO4,  (NH4)2HPO4,  K2HPO3,  Na2HPO3, 
(NH4)2HP03,  K2HAs04,  Na3AsO4,  K2C2O4, 
(NH4)2C204,  NaF,  and  K2CrO4+Aq.  With 
the  NH4  salts  the  decomposition  is  complete. 
(Dulong,  A.  ch.  82.  286.) 

Not  decomp.  by  alkali  sulphates +Aq. 
(Malaguti.) 

Precipitation  of  CaCO3  is  much  hindered 
by  alkali  citrates  or  metaphosphates. 


Solubility  in  K2SO4+Aq  at  25° . 


Sp..gr.  25°/250 

%  K2S04 

%  CaCO  3 

1.010 
1.021 
1.033 
1.048 
1.061 
1.069 
1.083 
1.084 

1.60 
3.15 
4.73 
6.06 
7.85 
8.88 
10.18 
10.48 

0.0104 
0.0116 
0.0132 
0.0148 
0.0168 
0.0192 
0.0192 
0.0188 

(Cameron    and    Robinson,    J.    phys.    Chem. 
1907,  11.  578.) 

The  solubility  of  CaCO3  in  Na2SO4+Aq 
in  equilibrium,  with  air  steadily  increases  with 
increasing  amounts  of  CaSO4  in  the  solution 
up  to  saturation  point  of  the  CaSO4.  In  the 
presence  of  solid  CaSO4  the  solubility  of 
CaCC3  is  much  decreased.  (Cameron  and 
Seidell,  J.  phys.  Chem.  1902,  6.  56.) 

See  under  CaH2(CO3). 

Solubility  in   Na2SO4-f  Aq  in  contact  with 
CO2  free  air  at  25°. 


Sp.  gr.  25°/25° 

%KC1 

%  CaC03 

g.  per  100  g.  H2O 

Na2SO,                                     CaCOs 

1.000 
1.024 
1.046 
1.072 
.092 
.101 
.122 
.133 
.179 

0.00 
3.90 
7.23 
11.10 
13.82 
15.49 
18.21 
19.84 
26.00 

0.0013 
0.0078 
0.0078 
0.0076 
0.0072 
0.0076 
0.0070 
0.0072 
0.0060 

0.97                             0.0151 
1.65                             0.0180 
4.90                             0.0262 
12.69                             0.0313 
14.55                             0.0322 
19.38                             0.0346 
23.90                             0.0360 

(Cameron,  Bell  and  Robinson,  J.  phys. 
1907,  11.  396.) 

Solubility  in  salts  +Aq. 

Ch. 

(Cameron   and    Robinson,    J.    phvs.    Chem. 
1907,  11.  578.) 

Solubility  in  NaCl+Aq  in  contact  with  CO2 
free  air  at  25°. 

g.  salt  added  per  litre 

mg.  CaO  dissolved 
per  litre 

Sp.  gr.  2o°/25° 

g.  per  100  g.  H2O 

0.000 

17.4 

NaCl 

CaC03 

0.  585  g.  NaCl 
1.17g. 
2.93g. 

20.05 
24.9 
31.1  ' 

.0079                  1.60 
.0314                  5.18 
.0466                  9.25 
.0734                11.48 
.0949                16.66 
.1346                22.04 
.1794                30.50 

O.C079 
O.C086 
O.C094 
0.0104 
0.0106 
0.0115 
0.0119 

0.85g.  NaNO3 
1.70 
4.25 

24.35 

27.7 
34.5 

0.805g.  Na2SO4,  10H,O 
1.61  g. 
4.03g. 

25.95 
31.15 
40.7 

(Cameron,  Bell  and  Robinson,  J.  phys.  Ch. 
1907,  11.  396.) 

Solubility  of  CaCO3  in  NaOH  +Aq. 

0.53g.  Na2CO3 
1.06g. 
2.65g. 

8.4 
7.2 
4.4 

Solvent 

1  litre  dissolves 

at  18° 

at  95°-100° 

H2O 
(a.  0.0001  n.  NaOH 
ca.  0.001    n.  NaOH 
ca.  0.01       n.  NaOH 

12.8  mg.  CaCOs 
8.7     " 
4.2     " 
4.3     " 

20.7  mg.  CaCOs 
9.6       "       " 
6.9       "       " 
5.7       "       " 

0.55g.  CaCl2,  6H2O 
l.lOg. 
2.75g. 

9.0 

8.4 
8.4 

a,e  Blanc,  Z.  anorg.  1906,  51.  185.) 

The  solubility  of  CaCO3  in  CO2-free  water 

CARBONATE,  CALCIUM  HYDROGEN 


183 


is   therefore   increased   by    the   addition   o 
NaCl,  NaNO3  or  Na2SO4,   10H2O,  but  de- 
creased by  the  addition  of  Na2CO3  or  CaCL 
6H20. 

(Gothe,  Ch.  Z.  1915,  39.  306.) 


Sol.  in  ferric  chloride  or  nitrate +Aq  with 
evolution  of  CO2  and  pptn.  of  Fe2O6H6  (Fuchs 
1831) ;  also  in  chlorides  or  nitrates  of  Al,  Mn 
Cr,  or  U,  but  not  in  FeCl2+Aq. 

Sol.  in  cold  SnCl4+Aq  with  pptn.  of  SnO2 

Insol.  in  cone.  Na2SO4,  MgSO4,  BaCl2 
MgCl2,  Pb(NO3)2,  or  AgNO3+Aq.  (Kar 
sten.) 

Abundantly  sol.  when  freshly  precipitatec 
in  CaCl2+Aq,  and  MgSO4+Aq.  (Hunt.) 

Absolutely  insol.  at  15-19°  in  BaO2H2  + 
Aq;  also  on  boiling. 

1  1.  H2O  containing  3-4  g.  MgSO4  dissolves 
1-2  g.  CaCO3,  and  als6  1  g.  MgCO3.  (Hunt 
Am.  J.  Sci  (2)  26.  109.) 

100  pts.  NaCl+Aq  (2.525%  NaCl)  dissolve 
0.0037  pt.  (calculated  as  CaO)  pptd.  CaCO3 
and  0.0053  pt.  calcspar.  (Lubavin,  J.  russ 
Soc.  24.  389.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch 
J.  1898,  20.  827.) 

Insol.  in  liquid  CO2.  (Biichner,  Z.  phys 
Ch.  1906,  64.  674.) 

Alcohol  dissolves  traces  of  CaCO3.  (Gris- 
chow.) 

Sol.  in  Na  citrate +Aq.     (Spiller.) 

Sol.  in  Ca  sucrate-j-Aq.    (Barreswill.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Insol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,43.314.) 

Amorphous.  Solubility  in  H20  cannot  be 
determined  because  of  its  instability.  (Ken- 
dall, Phil.  Mag.  1912,  (6)  23.  972.) 

Min.  Calcite.  In  contact  with  air  free  from 
CO2,  11.  H2O  dissolves  at: 


25°  50°  100° 

0.01433      0.01504      0.01779  g.  calcite. 

(Kendall,  Phil.  Mag.  1912,  (6)  23.  964.) 


In  contact  with  air  containing  3.7  pts.  C02 
per  10,000.  the  solubility  of  calcite  in  H2O 
was  found 'to  be  0.04608  g.  per  1.  at  25°  and 
0.02925  g.  per  1.  at  50°.  (Kendall,  Phil.  Mag. 
1912,  (6)  23.  973.) 

Min.  Aragonite.  In  contact  with  air  free 
from  C02,  1  1.  H2O  dissolves  at: 


25° 
0.01528 


50° 
0.01617 


100° 
0.01902  g.  aragonite. 

(Kendall,  Phil.  Mag.  1912,  (6)  23.  964.) 


+5H2O.    Efflorescent. 
+6H2O.    (Pelouze.) 

Calcium  hydrogen  carbonate,  CaH2(CO3)2. 
Known  only  in  aqueous  solution. 
CaCO3  dissolves  in  CO2+Aq. 


CaCO3  is  sol.  in  1428  pts.  H2O  sat.  with  CO2  at  0°, 
and  1136  pts.  at  10°.  (Lassaigne,  J.  ch.  med.  4.  312.) 

Bineau  could  dissolve,  even  in  large  quantities  of 
H2O  sat.  with  CO2,  only  */5  enough  CaCOs  to  form 


232. 

Chalk  dissolves  in  994.5  pts.  H2O  sat.  with  CO2, 
while  Iceland  spar  requires  3149  pts.  (Bischof.) 

CaCOs  is  sol.  in  1015  pts.  H2O  sat.  with  CO2  at  21° 
and  748.3  mm.  (Warington,  Chem.  Soc.  6.  296.) 

Solubility  of  CaCO3  in  CO2+Aq  at  p  pressure 
in  atmospheres.  CaO+CO2  =  mg.  C02 
and  CaO  dissolved,  corresponding  to 
CaC03=mg.  CaC03. 


P 

CaO  +C02 

CaC03  ' 

0.000504 

60.96 

74.6 

0.000808 

72.11 

85.0 

0.00333 

123 

137.2 

0.03187 

218.4 

223.1 

0.0282 

310.4 

296.5 

0.05008 

408.5 

360 

0.1422 

533 

0.2538 

1072 

663.4 

0.4167 

1500 

787.5 

0.5533 

1846 

885.5 

0.7297 

2270 

972 

0.9841 

2864 

1086 

(Schlosing,  C.  R.  74.  1522.) 


With  high  pressure,  1 1.  H2O  containing  CO2 
lissolves  at  most  3  g.  CaCO3.  This  maximum 
s  reached  at  5°  under  4  atmospheres'  pres- 
sure; at  10-13°  under  5  atmospheres;  and  at 
20°  under  7  atmospheres.  (Caro,  Arch. 
Pharm.  (3)  4.  145.) 

CaCO3  is  sol.  in  about  1000  pts.  H2C03  + 
A.q,  and  solubility  is  considerably  increased 
by  Na2SO4  or  MgSO4. 


000  pts.  H2O  sat.  with  CO2  dissolve  pts. 
Carrara  marble  at  t°,  and  B=  height  of 
barometer  in  millimetres. 


t° 

B 

Pts. 
CaCOs 

t° 

B 

Pts. 
CaCOj 

7.5 
8.5 
9.5 
20.5 
21.5 

754 
752 
754 
741 
744 

1.224 
1.202 
1.115 
0.975 
0.935 

22.0 
26.0 
26.5 
27.0 

28.0 

746 
740 
743 
741 
737 

0.920 
0.875 
O.$60 
0.885 
0.770 

Or,  from  7.5-9.5°,  1000  pts.  H2O  sat.  with 
CO2  dissolve  1.181  pts.  CaCO3;  from  20.5- 
22°;  0.9487  pt.  CaCO3;  from  26-28°,  0.855  pt, 
CaCO3. 

1S4 


CARBONATE,  CALCIUM  HYDROGEN 


Other  varieties  of  CaCOs  are  dissolved  as 
follows  in  1000  pts.  HfO  sat.  with  COS. 


\arunv 


Luneburg  chalk     .     . 

Pptd.  CaCOj    .     .     . 

Iceland  spar.     .     .     . 

Calcite 

Traversella  .... 

Dolomite,  semi-trans- 
parent   

Dolomite,  opaque,  in 
small  crystals     .     . 

Dolomite,  opaque,  in 
large  crystals     .     . 

Dolomite,  transparent, 
in  large  crystals 

Oolithic  limestone .     . . 

Dolomitic  limestone  . 


18 
IS 
18 
12 
12 

11.5 
11.5 
11 

11 
15 
15.5 


741) 
740 
735 
754 

754 

749 
755 
746 

749 
747 

740 


Pts. 


O.s3f> 
0.950 
1.970 

1.223 

.212 
0.654 
0.725 

.224 

1.073 

.252 
.573 


(Cossa,  Z.  anal.  8.  145.) 


Solubility  of  CaCOj  in  H*0  containing  COS 
at  various  pressures. 


CO-  pressure  in  at  in. 
Solubility 

(Engel,  C.  R.  1885,  101.  951.) 


1246 
1079   1403   1820  2109 


1  1.  H,O  dissolves  0.3850  g.  CaHs(CO3), 
at  15°.  (Treadwell,  Z.  anorg.  1898,  17.  186.) 

1 1.  of  sat.  CaHj(COs)j+Aq,  obtained  from 
pure  or  impure  limestone,  contains  1.13-1.17 

f.  CaCO8  at  15°.    (Treadwell,  Z.  anorg.  1898, 
7.  189.) 


Solubility  of  CaHj(CO8)2  in  H8O  containing 
CO,  at  15°. 


carbonic 
acid  in  gas 
at  0°  and 
760  mm. 

partial 
pressure 
mm. 

Free  car- 
bonic acid 
mg. 

CaH^Os)i 
in  100  cc.  of 
the  solution 

mg.  Ca 

8.94 

67.9 

157.4 

187.2 

46.2 

6.04 

45.9 

86.3 

175.5 

43.3 

5.45 

41.4 

52.8 

159.7 

39.4 

2.18 

16.6 

48.5 

154.0 

38.0 

1.89 

14.4 

34.7 

149.2 

36.8 

1  .  72 

13.1 

24.3 

133.1 

32.9 

0.79 

6.0 

14.5 

124  9 

30  8 

0.41 

3.1 

4.7 

82.1 

20.3 

0.25 

1.9 

29 

59.5 

14.7 

0.08 

0.6 

40.2 

9.9 

38  5 

9  5 

3s  f> 

9  5 

38  5 

9* 

(Treadwell  and  Reuter,  Z.  anorg.  1898,  17 
185.) 


1  1.  H>O  sat.  with  carbonic  acid  dissolves 
1.30  g.  CaC08  at  13.2°;  1  r>  g.  at  2,8 

^Treadwell.  /.  anon;.  1S9S.  17.  IS*U 

At  30°  C.  in  equilibrium  \\ith  the  aii,  not 
more  than  3  per  cent  of  the  ealeium  present 
is  eomhinetl  as  CaCOs.  At  lower  tempera- 
tures and  lesser  e.oneent  rat  ions  the  pereent- 
age  of  normal  earbonate  is  even  less,  aiul  prae- 
tieally  all  the  ealeium  present  is  eombimxl 
as  r'a  iUV  •...  (.Cameron  aiul  Briggs,  ,). 
phys.  (.'hem.  1901,  5.  549.) 

With  pressures  less  than  4.5  atmosMluMTs 
of  CO2  no  other  than  normal  ealeium  ear- 
bonate or  a  hydrate  of  the  normal  earbonate 
ean  exist  as  the  solid  phase  at  0°.  (.Cameron. 
J.  phys.  Chem.  191XS,  12.  560.) 

Solubility   in  H2O  in  eontaet   with  air,  con- 
taining TO;  with   varying  partial  pres- 
sures at  t°. 
P  =  partial  pressure  of  CO8. 


t-15° 


0.8 
1.5 
1.7 

O.S 
9.9 

13.0 
14.0 
31.6 


g.  per  1. 


0.193 
0.193 
0/J3S 
0.445 
0.627 
0.723 

o.oso 

l.ltfO 


t'Ov 


0.117 
0.152 
o  L35 

0  3-J7 

0.456 

o  ;>oo 

0.023 
1.117 


0.7 

1.6 

4.6 

7.8 

16.5 

30.1 

35.5 


K.  per  1. 


0.1 59 

0.177 
0.341 
0.440 
0  o39 
0.743 
0.755 


0.091 
0.111 

0/20S 
0.301 


O.S03 


t-40° 


06 
1.7 
2.9 
3.5 
7 

14.9 
22.2 
31.7 


g.  per  1. 


CnCO, 


0  130 
0.143 
0.175 
O.'JJVJ 
0.284 
0.3S4 
0.427 
0.4SO 


OOi 


0.07S 
O.OS5 
0.1(X> 
0.169 

0231 
0 . 293 
0.333 
0.470 


Similar  results  at  20°,  30°,  and  35°  are  also 

given. 

(Leather  and  Sen,  Mem.  Dept.  Agrie.  (India) 
Them.  Ser.  1909,  1.  117:  Seidell,  Solubil- 
ities, 1919.) 


CAKBOXATi;,  CALCIl.'M    HVDJiOr  ;K\ 


185 


Solubility  of  calcite  in  H2O  at  25°,  in  contact 
with  CO2  under  varying  pressures. 
P  =  approximate  pressure  of  CO2  in  atmos- 
pheres. 

Solubility  in    NaCl+Aq  at  25°  C.   and  in 
equilibrium  with  air. 

Ca(HCOah 

NaCI 

Grama 
per  liter 

Reacting  wt«. 
per  liter 

Grams 
per  liter 

Reacting 
wts.  per 
litre 

o.ooo" 

0.168 
0.362 
0.522 
0.872 
1.195 
1.695 
2.540 
4.040 
4.520 

P 

g.  per  1.  sat.  solution 

Solid  phase 

HzCOa 

Ca(HCOa): 

0.1046 
0.1770 

0.2051 
0.2152 
0.2252 
0.2212 
0.2172 
0.1971 
0.1569 
0.1227 

0.00065 
0.00110 
0.00128 
0.00134 
0.00140 
0.00138 
0.00135 
0.00123 
0.00095 
0.00076 

0.000 
9.720 

21.010 
30.301 
50.620 
69.370 
98.400 
147.400 
234.500 
262.300 

O.I 
1.1 
9.9 
13.2 

Hi  :; 

25.4 

0..22 
2.3 
20.0 
27.5 
34  1 
53.2 

0.67 
1.58 
3.62 
4.04 
4.21 
4.22 

CaCOa 
it 

t( 
ti 

Ca(HC03)2 

n 

(McCoy  and  Smith,  J.  Am.  Chem.  Soc.  1911, 
33.  468.) 

1  1.  H20  dissolves  2.3374  g.  CaCO,  at  5° 
under  a  CO2  pressure  of  2  atmos.  (Ehlert, 
Z.  Kl.'ktrpchem.  1912,  18.  727.) 

Solubility  data  for  calcite  in  H2O  contain- 
ing CO2,  with  and  without  the  presence  of 
salts  are  given  by  Seyler  and  Lloyd  (Chem. 
Sac,  1009,  96.  346.) 

A  critical  analysis  and  recalculation  of  re- 
sults of  Schloesing  and  others  is  given  by 
Johnston  (J.  Am.  Chem.  Soc.  1915,  37.  2001). 

CaCO 3  is  not  dissolved  by  CO2  and  H2O  in 
presence  of  MgCO3.  (Leather  and  Sen,  C.  A. 
1915.  181.) 

1  1.  of  1/10-normal  NaCl+Aq  dissolves 
0.3320  g.  CaH2(C03)2  at  15°.  (Treadwell 
and  Router,  Z.  anorg.  1898,  17.  193.) 


Solubility  of  CaH2(CO3)2  in  NaCl+Aq  sat. 
with  carbonic  acid  at  15°,  containing  5  g. 
NaCiperl/of  NaCl+Aq. 


'/.  carbonic 
ticid  in  j/as 
at  0°  and 

mrn.  11  v  - 
partial 

ftjfo, 

mg. 
CaHz(COah 
in  100  cc.  of 

cf 

7(50  mrn. 

pressure 

the  solution 

16.95 

128.8 

132.5 

218.4 

53.9 

11.47 

87.2 

110.1 

214.3 

52.9 

6.07 

46.1 

23.5 

149.2 

36.8 

3.16 

24.0 

13.5 

118.3 

29.2 

0.50 

3.8 

2.7 

73.9 

18.2 

0.41 

3.4 

0.3 

49.0 

12.1 

34.9 

8.6 

33.7 

8.3 

32.9 

8.1 

33.2 

8.2 

(Treadwell  and  Reuter,  Z.  anorg.  1898,  17. 
193.) 


(Cameron  and  Seidell,  J.  phys.  Chem.  1902, 
6.  51.) 

Solubility  in  various  salts +Aq  under  a  CO2 
pressure  of  2  atmos.  at  5°. 


Salt 

g.  salt  per 
lOOOg.  HzO 

g.  CaCOa  sol. 
in  1  1.  of  solvent 

H20 

2.3374 

MgCl2-f-6H2O 

6.08 
50.0 
86.0 
350.0 
700.0 
1150.0 
1725.0 
2300  (sat.) 

2.3518 
3.4045 
4.0826 
3  .  3009 
2.7357 
'      2.2054 
1.7058 
1.4060 

NaCI 

27  96 
50.0 
86.0 
106.9 
175.6 
263.4 
351  .'2 

3.2796 
3.7399 
3.7828 
3.6900 
3.3495 
2.8107 
2.  1625  at  8° 

MgS04+7H20 

105.3  (14°) 
sat.  at  14° 

2.1768 
0.91356 

Na2SO4  +  10H2O 

137. 
sat. 

7  (14°) 
at  14° 

1.4060 
1.9199 

(Ehlert  and  Hempel,  Z.  Elektrochem.  1912, 
18.  727.) 

Solubility  of  CaCO3  in  KCl+Aq  at  25°  sat. 
with  CO2  at  atmospheric  pressure. 

%  KCl 

%  CaCOa 

3.90 
7.23 
11.10 
13.82 
15.49 
18.21 
19.84     . 
26.00 

0.145 
0.150 
0.166 
0.165 
0.167 
0.154 
0.140 
0.126 

(Cameron   and   Robinson,    J.    phys.    Chem. 
1907,  11.  579.) 

186 


CARBONATE,  CALCIUM  COPPER  URANIUM 


Solubility  in  NaCl+Aq  in  contact  with  CO 
at  atmospheric  pressure  at  25°. 


g.  per  100  g.  H2O 


NaCl 


1.45 
5.69 
11.08 
15.83 
19.62 
29.89 
35.85 


CaC03 


0.150 
0.160 
0.174 
0.172 
0.159 
0.123 
0.103 


(Cameron,  Bell  and  Robinson,  J.  phys.  Ch 
1907,  11.  396.) 


Solubility  in  K2SO4+Aq,  sat.  with  CO2 
atmospheric  pressure  and  25°  temp. 


at 


%   S0.3 

%  CaO 

0.69 

0.69 

1.37 

0.69 

1.67 

0.47* 

2.18 

0.30* 

2.99 

0.24* 

*  Solid  phase,  CaSO4,  K2SO4. 

(Cameron  and  Robinson.) 

Solubility  in  Na2SO4+Aq  at  24°  in  equili- 
brium with  air. 


Total  Ca  calc. 
asCa(HC03)2. 
Grams  per  liter 

Ca  actually 
dissolved  as 
Ca(HCO3)2. 
Grams  per  liter 

Na2S04. 
Grams  per  liter 

0.0925 

0.0925 

0.000 

0.1488 

0.1488 

2.800 

0.1729 

0.1729  + 

5.235 

0.2330 

0.2210 

11.730 

0.3240 

0.3020 

36.860 

0.3960 

0.3440 

74.010 

0.4580 

0.3660, 

116.100 

0.5630 

0.3940 

184.200 

0.5910 

0.4060 

213.700 

0.6650 

0.4300 

255.900 

(Cameron  and  Seidell,  J.  phys.  Chem.  1902, 
6.  53.) 


Data  are  also  given  for  solubility  of  CaCO3 
in  NaCl+Na2SO4+Aq,  and  CaCO3+CaSO4 
in  NaCl+Na2SO4+Aq.  (Cameron,  Bell  and 
Robinson.) 


Calcium  copper  uranium  carbonate,  CaCO3 

3CuCO3,  4U(CO3)2+24H2O. 
Sol.  in  acids. 


Calcium  lead  carbonate,  zCaCO3,  */PbCO3. 
Min.  Plumbocalcite. 


Calcium  magnesium  carbonate,    CaCO3, 
MgC03. 

Min.  Dolomite.  1  1.  H2O  sat.  with  CO2  at 
18°  and  750  mm.  dissolves  0.31  g.  dolomite. 
(Cossa,  B.  2.  697.) 

Not  obtained  by  evaporating  solution,  but 
can  be  crystallized  from  CO2+Aq  between 
100°  and  200°.  (Hoppe-Seyler.) 

Dolomite  is  dissolved  by  CO2  and  H->O, 
but  solution  is  prevented  partially  by  CaCO3, 
and  wholly  by  MgCO3.  (Leather  and  Sen. 
C.  A.  1915.  181.) 

Insol.  in  cold  dil.  acids.  (Dolomieu,  J. 
Phys.  39.  1.) 

Insol.  in  cold  acetic  acid.    (Forchhammer.) 

Calcium  potassium  carbonate,  CaK2(CO3)2. 

Decomp.  by  H2O.  (Reynolds,  Chem.  Soc. 
1898,  73.  265;  Butschli,  C.  A.  1907,  2223). 

2CaCO3,  3K2CO3H-6H2O.    (Butschli.) 

Calcium  sodium  carbonate,  CaNa2(CO3)2. 
Anhydrous.    Decomp.  by  H20. 
+2H2O.     (Butschli,  C.  A.  1907.  2223.) 
+5H2O.     Min.   Gaylussite.    Sparingly  sol. 

in  H2O. 

Calcium  uranyl  carbonate,  CaCO3,  UO2C03  + 
20H2O. 

Min.  Liebigite.    Sol.  in  HCl-fAq. 

+zH2O.  Decomp.  by  H2O.  (Blinkoff, 
Dissert.  1900.) 

2CaO,  4UO3,  3C02+24H2O.  Decomp.  by 
H2O.  (Blinkoff,  Dissert.  1900.) 

Calcium  carbonate  chloride,  CaC03,  CaClo  + 
6H20. 

Sol.  in  H2O  with  immediate  decomp. 
(Fritzsche,  J.  pr.  83.  213.) 

Cerous  carbonate,  Ce2(C03)3+5,  and  9H2O. 
Insol.  in  H2O,  and  solution -of  CO2  in  H2O. 

(Vauquelin.) 

Somewhat  sol.  in  (NH4)2CO3+Aq.    (Jolin.) 
Insol.  in  neutral  salt  solutions  and  neutral 

alkali  carbonates +Aq;  easily  sol.  in  SO2  + 

Aq.    (Berthier,  A.  ch.  (3)  7.  77.) 

Ceric  carbonate,  Ce(CO3)2  +  3^H2O. 
Precipitate.    (Hisinger,  A.  ch.  94.  108.) 
Insol.   in  H2O.     Sol.   in  slight   traces  in 

Na2CO3+Aq;  si.  sol.  in  NaHCO3+Aq,  and 

n  (NH4)2C03+Aq.    (Rose.) 

Cerous  lanthanum  carbonate  fluoride. 

Min.  Batncesite,  Hamartite,  Hydrofluocerite. 
Slowly  decomp.  by  HCl-fAq,  easily  by 
H2SO4. 


carbonate,     Ce2(CO3)3, 


Cerous     potassium 
K2CO3+3H2O. 

Ppt.    (Jolin.) 

Ce2(CO3)3,  K2CO3  +  12H2O.    Ppt. 

Sol.    in    30%    K2CO3+Aq.      (Meyer, 
anorg.  1904,  41.  103.) 


Z. 


CARBONATE,  CUPRIC,  BASIC 


187 


Perceric  potassium  carbonate,  Ce2O3(CO3)3, 

4K2CO3  +  12H2O. 

Crystalline.  SI.  sol.  in  H2O  containing 
K2CO3;  sol.  in  dil.  H2SO4  with  decomp. 
(Job,  C.  R.  1899,  128.  1098.) 

Cerous    sodium    carbonate,    Ce2(CO3)3, 
2Na2CO3+2H2O. 

Ppt.    (Jolin.) 

2Ce2(CO3)3,  3Na2CO3+24H2Q(?).  Ppt. 
Easily  decomp.  (Meyer,  Z.  anorg.  1904,  41. 
103.) 

Chromous  carbonate,  CrCO3. 

Sol.  in  much  H2O;  si.  sol.  in  KHCO3+Aq. 
(Moberg,  J.  pr.  44.  328;  Moissan,  A.  ch.  (5) 
21.  199.) 

Chromic  carbonate,  basic,  Cr2O3,  2CO2. 

Precipitate.  (Parkmann,  Sill.  Am.  J.  (2) 
34.  321.) 

Cr2O3,  CO2+4H2O.  Insol.  in  H2O;  sol.  in 
acids;  when  freshly  pptd.  is  sol.  in  K2CO3,  or 
(NH4)2CO3+Aq,  and  still  more  sol.  in  KOH 
+Aq.  (Meissner.) 

Insol.  in  ethyl  acetate  (Naumann,  B. 
1910,  43.  314);  methyl  acetate.  (Naumann, 

B.  1909,  42.  3790.) 

2Cr2O3,  CO2+6H2O.  Precipitate.  (Lang- 
lois,  A.  ch.  (3)  48.  502.) 

Chromous   potassium  carbonate, 

CrC03,  K2C03  +  1^H20. 
Sol.  in  H2O  when  freshly  prepared;  slowly 
polymerizes;  stable  in  dry  air,  decomp.  in 
moist  air;  sol.  in  acids  with  decomp.    (Bauge, 

C.  R.  1898,  126.  1568.) 

Chromous  sodium  carbonate,  CrNa2(CO3)2  + 
H2O. 

Decomp.  when  heated.  In  Aq.  solution, 
passes  into  the  hydrate  containing  10  mols 
H2O.  (Bauge,  C.  R.  1897,  125.  1179.) 

+  10  H2O.  Very  sol.  in  cold  H2O;  Aq.  solu- 
tion decomp.  below  100°;  effloresces  in  the  air 
sol.  in  HCl+Aq  and  H2SO4+Aq.  (Bauge, 
C.  R.  1897,  125.  1178.) 

Cobaltous  carbonate,  basic,  5CoO,  2CO2-|- 
4H2O. 

Insol.   in   H2O;    sol.    in    (NH4)2SO4, 
(NH4)2CO3,  NH4NO3,  and  NH4Cl+Aq. 

Sol.  in  cold  NH4NO3,  and  NH4Cl+Aq 
(Brett,  1837.) 

Sol.  in  CO2+Aq,  and  acid  alkali  carbonates 
+Aq,  from  which  it  is  pptd.  on  boiling 
Very  si.  sol.  in  cone.  Na2CO3,  or  K2CO3+Aq 
largely  sol.  in  (NH4)2CO3+Aq,  and  partly  sol 
inNH4OH+Aq.  (Berzelius.) 

Not  pptd.  from  solutions  containing  Na 
citrate.  (Spiller.) 

4CoO,  CO2+4H2O.    Ppt.    (Beetz.) 

+3H2O.    (Meigen,  C.  C.  1905,  I.  1363.) 


Cobaltous  carbonate,  basic,  3CoO,  CO2  + 
2H2O. 

(Meigen,  C.  C.  1905,  I.  1363.) 

3H2O.    (Rose,  Pogg.  84.  551.) 

3CoO,  2CO2+4H2O.  (Bratin,  Z.  anal.  6. 
76.) 

2CoO,  CO2+3^H2O.  Converted  into 
5CoO,  2CO2+4H2O  by  H2O.  (Beetz.) 

Cobaltous  carbonate,  CoCO3. 

Anhydrous.  Not  attacked  by  cold  cone. 
HC1,  or  HNO3+Aq.  (Senarmont,  A.  ch.  (3) 
30.  129.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  827.) 

Min.  Sphcerocobaltite.  SI.  attacked  by  cold 
HNO3,  or  HCl+Aq. 

+2/3H2O.  Sol.  in  acids.  (Deville,  A.  ch.  (3) 
33.  95.) 

+6H2O.    (Deville.) 

Decomp.  by  H2O  with  formation  of  a  basic 
carbonate.  (Berzelius.) 

Cobaltous  potassium  carbonate,  CoCO3, 
K2CO3+4H2O. 

Decomp.  by  H2O.  (Deville,  A.  ch.  (3)  33. 
90.) 

Ppt.  Decomp.  by  H2O.  (Reynolds,  Chem. 
Soc.  1898,  73.  264.) 

CoCO3,  KHCO?+4H2O.  Decomp.  by 
H2O.  (Deville.) 

Cobaltous  sodium  carbonate,  CoCO3,  Na2CO3 

+4H2O,  and  10H2O. 
Decomp.  by  H2O.    (Deville,  A.-ch.  (3)  33. 

75.) 

Cupric  carbonate,  basic. 

The  compounds  produced  by  pptn.  of 
copper  solutions  by  carbonates  are  unstable 
and  possess  varying  solubilities  in  solutions 
of  C02.  On  treatment  with  solutions  of  CO2, 
these  substances  pass  over  into  an  apparently 
stable  compound  possessing  a  definite  solu- 
bility in  solutions  of  CO2  of  definite  concen- 
tration, which  solubility  increases  with  the 
concentration  of  CO2.  Solubility  of  this 
compound  in  various  salts +Aq  is  recorded. 
(Free,  J.  Am.  Chem.  Soc.  1908,  30.  1374.) 

8CuO,  CO2+5H2O.  (Deville,  A.  ch.  (3) 
33.  75.) 

6CuO,  CO2.    (Field,  Chem.  Soc.  14.  70.) 

3CuO,  CO2+2H2O.  (Favre,  A.  ch.  (3)  10. 
119.) 

5CuO,  2CO2+6H2O.    (Struve.) 

2CuO,  CO2+H2O.  Insol.  in  H2O;  easily 
sol.  in  acids,  even  H2SO3+Aq;  si.  sol.  in 
H2CO3+Aq,  30,720  pts.  of  the  solution  con- 
taining 1  pt.  CuO.  (Jahn.)  Sol.  in  4690  pts. 
H2CO3+Aq  sat.  at  4-6  atmos.  pressure. 
(Wagner.)  Sol.  in  3833  pts.  sat.  H2C03+Aq. 
(Lassaigne,  J.  ch.  med.  4.  312.) 

Sol.  in  NH4  salts+Aq.  Partially  sol.  in 
Na2CO3,  or  K2CO3+Aq,  and  more  sol.  in 


188 


CARBONATE,  COPPER  POTASSIUM,  BASIC 


NaHCO3,  or  KHCO3+Aq;  sol.  in  (NH4)2CO3 
+Aq.  (Favre,  A.  ch.  (3)  10.  18.) 

Less  sol.  in  (NH4)2CO3+Aq  than  CuO  in 
NH4OH+Aq.  (Thomson,  1831.)  Sol.  in 
KCN+Aq.  (Berzelius.)  Sol.  in  NH4C1,  or 
NH4NO3+Aq.  (Brett.) 

Sol.  in  ferric  salts  with  pptn.  of  Fe2O6H6. 

Insol.  in  liq.  NH3.  (Franklin  and  Kraus, 
Am.  Ch.  J.  1898,  20.  827.) 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,43.314.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Sol.  in  ethyl  amine  carbonate +Aq. 
(Wurtz.) 

Sol.  in  cane  sugar +Aq.  (Peschier,  Repert. 
1820,  6.  85.) 

Not  pptd.  from  solutions  containing  sodium 
citrate.  (Spiller.) 

Insol.  in  pvridine.  (Schroeder,  Dissert. 
1901.) 

Min.  Malachite.  Sol.  in  acids,  and  NH4OH 
+Aq. 

+2H2O.    (Favre.) 

8CuO,  5CO2+7H2O.  (Groger,  Z.  anorg. 
1900,  24.  137.) 

3CuO,  2CO2+H2O.  Insol.  in  H2O.  Sol. 
in  NH4OH+Aq,  also  in  hot  cone.  NaHCO3  + 
Aq. 

Min.  Azwite. 

Copper  potassium  carbonate,  basic,  8CuO, 
2K2CO3,  7CO2+17H20. 

Ppt.;  decomp.  by  H2O.  (Groger,  B.  1901, 
34.  430.) 

Mixture.  (Wood  and  Jones,  C.  A.  1907. 
2667). 

5CuO,  4CO2,  K2CO3+10H2O.  Decomp. 
by  H2O.  (DeviUe,.A.  ch.  (3)  33.  102). 

Cupric  potassium  carbonate,  CuCO3,  K2CO3. 

Decomp.  by  H2O.  (Wood  and  Jones,  C.  A. 
1907.  2667.) 

+H2O.     (Wood  and  Jones.) 

+4H2O.  Decomp.  by  H2O.  (Reynolds, 
Chem.  Soc.  1898,  73.  263.) 

Could  not  be  obtained.    (Wood  and  Jones.) 

2CuCO3,  K2CO3  +4H2O.  Decomp.  by  H2O. 
'(Wood  and  Jones.) 

Cupric  sodium  carbonate,  CuCO3,  Na2CO3. 

Not  decomp.  by  cold  H2O.  (Debray,  C  R 
49.  218.) 

+3H2O. 

Cupric  zinc  carbonate,  2CuO,  3ZnO,  2CO2  + 

3H2O,  or  3CuO,  9ZnO,  4CO2+8H2O. 
Min.  Aurichalcite.    Easily  sol.  in  HC1  +  Aq. 

Cupric  carbonate  ammonia  (cuprammonium 

carbonate),  CuCO3,  2NH3. 
Decomp.  by  H2O.     Insol.  in  alcohol  and 
ether.    Sol.  in  (NH4)2CO3+Aq.     (Favre,  A. 
•ch.  (3)  10.  116.) 


Didymium  carbonate,  Di2(CO3)3+H2O,  or 
6H20. 

Insol.  in  H2O.  Only  traces  dissolve  in  CO2 
+Aq.  Insol.  in  solutions  of  alkali  carbonates 
or  bicarbonates-f-Aq.  (Marignac,  A.  ch.  (3) 
38.  166.)  Very  si.  sol.  in  cone.  NH4Cl+Aq. 
(Rose.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

+8H2O.    (Cleve,  Bull.  Soc.  (2)  43.  363.) 


Didymium  potassium  carbonate,  Di2(CO3)3, 
K2C03+4H20. 

Insol.  in  H2O.     (Cleve,  Bull.  Soc.  (2)  43. 
363.) 

+  12H2O.    (Cleve.) 


Didymium    sodium    carbonate,    2Di2(COsK 

3Na2CO3+9H2O. 
Ppt.    (Cleve.) 
Di2(CO3)3,2Na2CO3+8H2O.  Ppt.  (Cleve.) 


Dysprosium  carbonate,  Dy2(CO3)3+4H2O. 
Insol.   in   H2O.      (Jantsch,    B.    1911,    44. 

1277.) 


Erbium  carbonate,  Er2O3,  2C02+2H2O. 
Insol.  in  H2O.    (Hoglund.) 


Erbium    sodium    carbonate,    Er2(CO3)3, 

5Na2CO3+36H2O. 
Efflorescent.    Decomp.  by  H2O. 

Gadolinium  carbonate,  basic,  Gd(OH)CO3  + 
H2O. 

Ppt.    (Benedicks,  Z.  anorg.  1900,  22.  417.) 

Glucinum  carbonate,  basic,  3G1O,  CO2;  4G1O, 

C02;  5G10,  C02+5H20,  etc. 
Not  perceptibly  sol.  in  H2O  or  H2CO3+Aq. 
Decomp.  by  boiling  H2O.  Easily  sol.  in  acids. 
Sol.  in  NH4  salts,  and  KOH,  or  NaOH+Aq. 
Sol.  in  alkali  carbonates,  especiallv 
(NH4)2CO3+Aq.  (Vauquelin.)  SI.  sol.  in 
K2CO,+Aq.  When  solution  in  (NH4)2CO3 
is  boiled,  a  more  basic  carbonate  is  pptd. 
(Rose.) 


Glucinum  carbonate,  G1C03+4H2O. 

Efflorescent.  Sol.  in278pts.  H2O.  (Klatzo, 
J.  pr.  106.  242.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 

No  definite  carbonate  of  glucinum  exists. 
(Cameron,  J.  phys.  Chem.  1908, 12.  572.) 


CARBONATE,  LANTHANUM 


189 


Glucinum    potassium 
2K2CO3. 


carbonate,     3G1C03, 


Easily  sol.  in  H2O,  but  decomp.  by  boiling. 
(Debray.)  Less  easily  sol.  in  alcohol. 

Indium  carbonate,  In2(CO3)3. 

Ppt.  Insol.  in  K2CO3,  or  Na2CO3-f-Aq. 
Sol.  in  (NH4)2CO3+Aq.  (Winkler,  J.  pr. 
94.  1.) 

Iron  (ferric)  carbonate,  basic. 

9Fe2O3,  CO2  +  12H2O.  (Wallace,  Chem. 
Gaz.  1858.  410.) 

3Fe2O3,  CO2+4H2O,  and  8H2O.  (Barrat, 
C.  N.  1.  110.) 

+6H2O.    (Wallace.) 

2Fe203,  C02  +  1KH20.  (Rother,  Pharm. 
J.  Trans.  (3)  4.  576.) 

Fe2O3,  CO2.  (Parkmann,  Sill.  Am.  J.  (2) 
34.  321.) 

These  and  other  similar  basic  salts  are  ppts., 
easily  decomp.  on  standing  into  Fe2O6H6. 

Iron  (ferrous)  carbonate,  FeCO3. 

Insol.  in  H2O. 

Sol.  in  acids,  even  in  H2CO3+Aq. 

See  Carbonate,  ferrous  hydrogen. 

Min.  Siderite,  Spathic  ore.  SI.  attacked  by 
dil .  acids .  Sol .  in  H  2CO  3 + Aq  under  pressure . 

Insol.  in  NH4C1,  or  NH4NO3+Aq.    (Brett.) 

+H2O.  SI.  sol.  in  H2O;  easily  sol.  in  acids: 
sol.  inH2CO3+Aq. 

Sol.  in  NH4C1 + Aq .  Sol.  in  ferric  salts  +  Aq 
with  evolution  of  CO2  and  pptn.  of  Fe2O6H6. 

Soluble  in  an  aqueous  solution  of  cane  sugar. 

Solubility  in  salts+Aq  free  from  CO2. 


Salt 

g.  salt  per  1000 
g.  H20 

1  1.  of  solvent 
dissolves 
g.  FeCOa 

NaCl 

351.2 

0.35042 

MgCl2  + 
6H2O 

2300.0 

4.2049 

Na2SO4 
+  10H2O 

137.7 

sat.  at  +14° 

0.70085 
0.93444 

MgS04+ 
7H2O 

105.3 

sat.  at  +18° 

1.4667 
2.9334 

(Ehlert,  Z.  Elektrochem.  1912,  18.  728.) 

Iron  (ferrous)  hydrogen  carbonate, 

FeH2(C03)2(?). 

Known  only  in  aqueous  solution. 

By  conducting  CO2  at  ordinary  pressure 
through  H2O,  in  which  Fe  is  suspended,  a  solu- 
tion containing  9.1  pts.  FeCO3  to  10,000  pts. 
H2O  is  obtained,  (v.  Hauer,  J.  pr.  81.  391.) 


100  pts.  H2CO3+Aq  dissolve  0.72  pt. 
FeC03.  (Wagner.) 

FeCO3  dissolves  in  1381  pts.  H2O  saturated 
with  CO2,  under  a  pressure  of  4-6  atmos- 
pheres. (Wagner,  J.  B.  1867.  135.) 

1  1.  H2O  dissolves  6.1907  g.  FeCO3  (pure) 
under  a  CO2  pressure  of  2  atmos.  (Ehlert, 
Z.  Elektrochem.  1912,  18.  728.) 

Solubility  in  various  salts+Aq  in  presence  of 
CO2  under  pressure  of  2  atmos. 


Salt 

With  COz  of  2  atmos.  pressure 

g.  salt  per  1000 
g.  H20 

1  1.  of  solvent 
dissolves 
g.  FeCCh 

H20 

6.1907 

NaCl 

50 

106.9 
175.6 
263.4 
351.2 

— 

MgCl2  + 
6H2O 

86.9 
700.0 
1150.0 
1437.5 
1725.0 
2300.0 

5.8403 
4.5553 
4.4587 
4.6934 
5.3975 
9.0524 

Na2SO4 
+  10H2O 

137.7 

sat.  at  +14° 

7.9428 
9.5780 

MgS04  + 
7H2O 

105.3 

sat.  at  +18° 

6.2423 
7.3922 

(Ehlert,  Z.  Elektrochem.  1912,  18.  728.) 

A  bicarbonate  of  ferrous  iron  is  not  formed 
under  pressures  of  CO2  up  to  5  atmospheres 
at  0°.     (Cameron,  J.  phys.  Chem.  1908,  12. 
571.) 

Iron  (ferrous)  magnesium  carbonate,  FeCO3, 
Mo-rn, 

Min.  Pistomesite. 

FeCO3,  2MgCO3.     Min.  Mesitite. 

Iron  (ferrous)  potassium  carbonate, 

FeK2(CO3)2+4H2O. 

Ppt.    Decomp.  by  H2O.    (Reynolds,  Chem. 
Soc.  1898,  73.  265.) 


Lanthanum    carbonate,    La2(CO8)3-f-H2O, 
3H2O,  and  8H2O. 

Insol.  in  H2O.     CO2+Aq  dissolves  traces. 
Insol.  in  (NH4)2CO3+Aq. 

Insol.  in  acetone.    (Naumann,  B.  1904,  37. 
4329.) 

Min.  Lanthanite. 


190 


CARBONATE,  LANTHANUM  POTASSIUM 


Lanthanum  potassium  carbonate,  La2(COs)3, 

K2CO3  +  12H2O. 

Sol.  in  30%  K2CO3+Aq.  (Meyer,  Z. 
anorg.  1904,  41.  101.) 

Lanthanum  sodium  carbonate,  2La2(CO3)3, 

3Na2CO3+20H2O(?). 

Ppt.  Easily  decomp.  (Meyer,  Z.  anorg. 
1904,  41.  102.) 

Lead  carbonate,  basic,  2PbCO3,  PbO2H2; 
5PbCO3,  3PbO2H2;  3PbCO3,  PbO2H2; 
5PbCO3,  PbO2H2. 

Whit"  Le~d.  Insol.  in  H2O.  Nearly  insol. 
in  H2CO3+Aq,  even  under  pressure.  Sol.  in 
dil.,  insol.  in  cone.  KOH+Aq.  Insol.  in 
normal,  or  acid  alkali  carbonates  + Aq .  (Bott- 
ger.) 

Sol.  in  cold  dil.  NH4Cl+Aq.    (Brett.) 

PbCO3,  PbO2H2.  Very  si.  sol.  in  H2O. 
(Yorke.) 

2PbCO3,  PbO2H2. 

Solubility  is  less  than  O.OC02  millimol  Pb 
in  1  liter  H2O  at  18°.  (Pleissner,  C.  C.  1907, 
II.  1056.) 

When  not  exposed  to  air,  sol.  in  32,000 
pts.  (NH4)2SO4+Aq  (0.2  g.  per  1.);  26,000 
pts.  KNO3+Aq  (0.2  g.  per  1.);  23,000  pts. 
CaCl2+Aq  (0.2  g.  per  1.);  4600  pts.  NH4NO3 
+Aq  (0.2  g.  per  1.);  4300  pts.  H2O  sat.  with 
CO2. 

When  exposed  to  air  in  beakers,  sol.  in 
43,000  pts.  (NH4)2SO4+Aq  (0.2  g.  per  1.); 
43,000  pts.  KNO3+Aq  (0.2  g.  per  1.);  26,000 
pts.  CaCl2+Aq  (0.2  g.  per  1.);  26,000  pts. 
NH4NO3+Aq  (0.2  g.  per  1.);  4300  pts.  H2O 
sat.  with  CO2  (0.2  g.  per  1.).  (Muir,  Chem. 
Soc.  31.  664.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

3PbO,4PbCO3+2H2O.  Ppt.  (Stromholm, 
Z.  anorg.  1904,  38.  446.) 

Lead  carbonate,  PbCO3. 

Sol.  in  50,551  pts.  H2O  at  ordinary  temp. 

Sol.  in  23,450  pts.  H2O  with  little  ammo- 
nium acetate,  carbonate,  and  free  ammonia; 
and  in  somewhat  less  H2O,  containing  much 
ammonium  nitrate  with  carbonate  and  free 
ammonia.  (Fresenius,  A.  69.  124.) 

Calculated  from  electrical  conductivity  of 
PbCO3+Aq,  1  1.  H2O  dissolves  3  mg.  PbCO3 
at  10°.  (Kohlrausch  and  Rose,  Z.  phys.  Ch. 

Solubility  is  0.0002  millimol.  Pb  in  1  liter 
H2O  at  18°.  (Pleissner,  C.  C.  1907,  II.  1056.) 

SI.  sol.  in  H2O.  1.5  x  10-3  g.  are  contained 
in  1  1.  of  sat.  solution  at  20°.  (Bottger,  Z 
phys.  Ch.  1903,  46.  604.) 

Easily  sol.  in  acids,  even  HC2H3O2;  but  not 
decomp.  by  cone.  HNO3+Aq  on  account  of 
insolubility  of  Pb(NO3)2  in  HNO3+Aq.  In- 
sol. in  a  mixture  of  1  pt.  H2SO4  and  6  pts. 
absolute  alcohol,  or  in  an  alcoholic  solution 
of  racemic  or  tartaric  acids. 


Insol.  in  H2CO3+Aq.  (Jahn,  A.  28.  117.) 
Very  si.  sol.  in  H2CO3+Aq,  but  solution  is 
prevented  by  traces  of  various  salts.  (Tiin- 
nerman.)  Sol.  in  7144  pts.  sat.  H2CO3+Aq. 
(Lassaigne,  J.  ch.  med.  4. 312.)  H2O  sat.  with 
CO2  under  4-6  atmos.  pressure  dissolves  only 
traces  of  Pb;  1000  pts.  of  solution  containing 
0.5  pt.  PbCO3.  (Wagner,  Z.  anal.  6.  167.) 

Solubility  of  PbCO3  in  H2CO3+Aq  at  18°. 


mg.  per  1. 


C02 


0 

2.8 

5.4 

14.4 

26 

43.5 
106 


PbCO* 


1.75 

6 

7 

8.2 

9.9 
10.9 
15.4 


(Pleissner,  C.  C.  1907,  II.  1056.) 

Sol.  in  NH4C2H3O2+Aq,  and  NH4Cl+Aq. 
(Weppen,  1837.)  Sol.  in  KOH+Aq;  not  ab- 
solutely insol.  at  ord.  temp,  in  an  excess  of 
K2CO3,  or  Na2CG3+Aq,  and  still  more  sol.  at 
100°;  but  absolutely  insol.  in  NaHC03, 
KHCO3,  or  (NH4)2CO3+Aq.  (Rose.)  Insol. 
in  NH4OH+Aq;  sol.  in  KOH  or  NaOH+Aq; 
decomp.  by  boiling  Ca(NO3)2+Aq.  (Berze- 
lius.) 

SI.  decomp.  (Persoz),  not  at  all  decomp. 
(Malaguti)  by  alkali  sulphates +Aq. 

Partially  decomp.  by  boiling  with  K2SO4, 
Na2S04,  (NH4)2S04,  CaSO4,  MgSO4, 
Na2HPO4,  NaNH4HPO4,  K2SO3,  Na2SO3, 
(NH4)2SO3,  Na2HPO3,  Na2B4O7,  K3As04, 
Na3AsO4,  K2C2O4,  Na2C2O4,  NaF,  and 
K2CrO4+Aq.  With  the  NH4  salts,  the 
decomp.  is  complete.  (Dulong,  A.  ch.  82. 
290.) 

Easily  sol.  in  hot  NH4Cl+Aq.  (Brett; 
Rose.) 

When  1  mol.  PbCO3  is  boiled  with  1  mol. 
K2C2O4,  15%  of  the  PbCO3  is  decomp.;  with 
1  mol.  K2CO3,  93.28%  is  decomp.  (Mala- 
guti.) 

Not  decomp.  by  K2SO4+Aq.  (Rose.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,^20.828.) 

Sol.  in  an  aqueous  solution  of  acetates. 
(Mercer,  1844.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Not  pptd.  in  presence  of  Na  citrate. 
(Spiller.) 

Min.  Cerussite. 

Lead  sodium  carbonate,  4PbCO3,  Na2CO3. 
Insol.  in  H2O.    (Berzelius,  Pogg.  47.  199.) 

Lead  carbonate  bromide,  PbCO3,  PbBr2. 
Insol.  in  H2O.    (Storer's  Diet.) 


CARBONATE,  LITHIUM 


191 


Lead  carbonate  chloride,  PbCO3,  PbCl2. 
Insol.  in  H2O.     (Miller,  Chem.  Soc.  (2)  8. 

37.) 

Min.  Phosgenite.    Easily  sol.  in  acids. 

Lead  carbonate  iodide,  PbCO3,  PbI2. 
Insol.  in  H2O.    (Poggiale.) 


(Tschugaeff,  Z.  anorg.  1914,  86.  159.) 

Sat.  solution  boils  at  102°.     (Kremers.) 
More  sol.  in  CO2+Aq  than  in  H2O.     100 


pts.  sat.  CO2+Aq  dissolve  5.25  pts.  Li2CO3. 
(Troost.)    See  LiHCO3. 
Sol.  in  NH4  salts +Aq. 

Solubility  in  salts -f-Aq  at  25°. 

C  =  concentration   of   salt   solution  in   g.- 
equiv.  per  1. 

S  =  solubility  of  Li2CO3  in  g.-equiv.  per  1. 


Lead  carbonate  sulphate,  PbCO3,  PbSO4. 
Min.  Lanarkite.     Sol.  in  HNO3+Aq  with 
residue  of  PbSO4. 
3PbCO3,    PbSO4.      Min.    LeadhilLite.     As 
above. 

Lithium  carbonate,  Li2CO3. 
100  pts.  H2O  dissolve  1  pt.  Li2CO3.    (Vau- 
quelin,  A.  ch.  7.  284.) 
100  pts.   H2O    at    13°   dissolve  0.769   pt. 
Li2CO3;  at  102°,  0.778  pt.  Li2CO3.    (Kremers, 
Pogg.  99.  48.) 
100  pts.  H2O,  cold  or  hot,  dissolve  1.2  pts. 
Li2CO3.     (Troost,  A.  ch.  (3)  61.  103.) 
100  pts.  HoO  dissolve  1.4787  pts.  at  15°, 
0.7162  pt.  at  100°.     (Draper,  C.  N.  56.  169.) 

100  pts.  H2O  dissolve  pts.  Li2CO3  at  t°. 

Salt 

C 

s 

KNO3 

0.25 
0.50 
0.75 
1.00 
1.50 
2.00 

0.3647 
0.3688 
0.3676 
0.3656 
0.3490 
0.3268 

KC1 

0.10 
0.25 
0.50 
0.75 
1.00 
1.50 
2.00 

0.3553 
0.3590 
0.3782 
0.3832 
0.3835 
0.3731 
0.3558 

NaCl 

0.10 
0.25 
0.50 
0.75 
1.00 
1.50 
2.00 

0.3569 
0.3691 
0.3867 
0.3956 
0.3946 
0.3901 
0.3776 

t°              Pts.  LixCOi               t°             Pts.  Li2CO3 

0             1.539              75             0.866 
10             1.406            100             0.728 
20             1.329             102             0.796 
50             1  .  181 

K2SO4 

0.25 
0.50 
1.00 

0.4028 
0.4356 
0.4860 

2 

0.796  pt.  is  dissolved  at  102°  in  less  than 
J4  hour,  and  0.955  in  1  hour.     (Beketow,  J. 
russ.  Soc.  1884.  591.) 
Sat.  solution  at  15°  has  sp.  gr.  1.014,  and 
contains  1  g.  Li2CO3  to  70  g.  H2O,  while  solu- 
tion sat.  at  0°  has  sp.  gr.  1.0168  and  contains 
1  g.  Li2CO3  in  64.6  g.  H2O.     By  long  spon- 
taneous evaporation  at   15°  a  solution  can 
be  obtained  of  1.0278  sp.  gr.  containing  1  g. 
Li2CO3  in  45.57  g.  H2O.     (Fliickiger,  Arch. 
Pharm.  (3)  25.  549.) 
By  boiling  for  an  instant  with  H2O  a  solu- 
tion is  obtained,  which  has  sp.  gr.  1.0074  and 
contains  1  g.  Li2CO3  to  139  g.  H2O.    (Fliicki- 
ger,  Arch.  Pharm.  (3)  26.  543.) 
0.1687  mol.  is  sol.  in  1  1.  H2O  at  25°.    (Roth- 
mund,  Z.  phys.  Ch.  1909,  69.  531.) 
Sat.  Li2CO3+Aq  contains  at: 

95°              75° 
0.723          0.833%  by  wt.  Li2CO3. 

Na2SO4 

0.50 
1.00 
2.00 

0.4411 
0.4926 
0.5534 

2 

NH4C1 

0.10 
0.25 
0.50 
0.75 
1.00 
1.50 
2.00 
4.00 

0.3902 
0.4677 
0.5659 
0.6270 
0.6810 
0.7463 
0.7739 
.  0.7881 

(NH4)2S04 

0.25 
0.50 
1.00 
1.50 
2.00 

0.5059 
0.7863 
0.9804 
1.109 
1.174 

2 

KC103 

0.1 
0.2 
0.4 

0.3500 
0.3570 
0.3616 

(Geffcken,  Z.  anorg.  1905,  43.  198.) 

• 

Insol.  in  liquid  NH3.     (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 


192 


CARBONATE,  LITHIUM  HYDROGEN 


Solubility  in  organic  compds.  +Aq  at  25°. 
Solubility  in  H2O  at  25°  =0.1687  mols.  litre. 

Solubility  in  organic  compds.  +Aq. 
at  25°—  -Continued. 

Organic  compd. 

Normality  of 
the  solution 

Mol.  Li2C03 
sol.  in  1  1. 

Organic  compd. 

Normality  of 
the  solution 

Mol.  Li2C03 

sol.    in  1  1. 

Methyl  alcohol 

0.250 
0.5 
1.0 

0.1604 
0.1529 
0.1394 

Thio-urea 

0.125 
0.250 
0.5 
1.0 

0.1667 
0.1643 
0.1600 
0.1523 

Ethyl  alcohol 

0.125 
0.250 
0.5 
1.0 

0.1614 
0.1555 
0.1417 
0.1203 

Dimethyl-pyrone 

0.125 
0.250 
0.5 
1.0 

0.  1562 
0-.  1460 
0.1284 
0.0992 

Propyl  alcohol 

0.125 
0.250 
0.5 
1.0 

0.1604 
0.1524 
0  .  1380 
0.1097 

Ammonia 

0.125 
0.250 
0.5 
1.0 

0.1653 
0.1630 
0.1577 
0.1466 

Tertiary  amyl 
alcohol 

0.125 
0.250 
0.5 
1.0 

0.1564 
0.1442 
0.1224 
0.0899 

Diethylamine 

0.125 
0.250 
0.5 
1.0 

0.1589 
0.1481 
0.1283 
0.0937 

Acetone 

0.125 
0.250 
0.5 
1.0 

0.1600 
0.1515 
0.1366 
0.1104 

Pyridine 

0.125 
0.250 
0.5 
1.0 

0.1592 
0.1503 
0.1347 
0.1091 

Ether 

0.125 
0.250 
0.5 

0.1580 
0.1476 
0.1300 

Piperidine 

0.125 
0.250 
0.5 
1.0 

0.1584 
0.1488 
0.1320 
0.1009 

Formaldehyde 

0.125 
0.250 
0.5 
1.0 

0.1668 
0.1653 
0.1606 
0.1531 

Urethane 

0.125 
0.250 
0.5 
1.0 

0.1604 
0.1525 
0.1377 
0.1113 

Glycol 

0.125 
0.250 
0.5 
1.0 

0.1660 
0.1629 
0.1565 
0.1472 

Acetamide 

0.250 
0.5 
1.0 

0.1614 
0.1520 
0.1358 

Glycerine 

0.125 
0.250 
0.5 
1.0 

0.1670 
0.1647 
0.1613 
0.1532 

Acetonitrile 

0.125 
0.250 
0.5 
1.0 

0.1618 
0.1556 
0.  1429 
0.1178 

Mannitol 

0.125 
0.250 
0.5 

0.1705 
0.1737 
0.1778 

Mercuric  cyanide 

0.125 
0.250 

0.1697 
0  .  1704 

Glucose 

'0.125 
0.250 
0.5 
1.0 

0.1702 
0.1728 
0.1752 
0.1778 

(Rothmund,  Z.  phys.  Ch.  1909,  69.  531.) 

Insol.  in  methyl  acetate.      (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.      (Naumann, 
B.  1904,  37.  3601.) 
Insol.  in  acetone.    (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Lithium  hydrogen  carbonate,  LiHCOs. 
100  pts.  H2O  dissolve  5.501  pts>  at  13°. 
(Bewad,  B.  17.  406  R.) 

Sucrose 

0.125 
0.250 
0.5 
1.0 

0.1693 
0.1689 
0.1661 
0.1557 

Urea 

• 

0.125 
0.250 
0.5 
1.0 

0.1686 
0.1673 
0.1643 
0.1605 

CARBONATE,  MAGNESIUM 


193 


Magnesium  carbonate,  basic,  Mg3C2O7+ 
3H2O  =3MgO,  2CO2+3H2O  or  2MgC03, 
MgO2H2+2H2O.  (Fritzsche,  Pogg.  37. 
310.) 

Magnesia  alba,  3MgCO3,  Mg(OH)2  + 
4H20,  4MgG03,  Mg(OH)2+5H20,  or 
5MgC03,  2Mg(OH)2+7H20. 

Very  si.  sol.  in  H?O.  Sol.  in  10,000  pts. 
hot  or  cold  H20.  (Bineau.) 

Sol.  in  2500  pts.  cold,  and  9000  pts.  hot 
H20.  (Fyfe.) 

Sol.  in  H2Q  containing  CO2. 

Very  easily  sol.  in  acids. 

Easily  sol.  in  dil.  HCl+Aq. 

Easily  sol.  in  NH4  sulphate,  nitrate,  or  suc- 
cinate+Aq,  also  in  (NH4)2C03+Aq.  (Witt- 
stein.)  Sol.  in  cold  Na2CO3,  K2C03,  K2S04, 
KC1,  or  KNO3+Aq  (Longchamp);  also  in 
NH4Cl+Aq,  separating  out  on  heating. 
(Vogel,  J.  pr.  7.  455.)  Slowly  sol.  in  cone. 
BaCl2,  CaCl2,  or  ZnSO4+Aq.  (Karsten.) 

Sol.  in  MgSO4+Aq.    (Dulong.) 

Sol.  in  ferric  salts +Aq  with  evolution  of 
C02  and  pptn.  of  Fe206H6.  (Fuchs.) 

Sol.  in  boiling  Co,  Ni,  Zn,  Mn,  or  Cu 
nitrates  or  chlorides +Aq. 

Min.  Hydromagnesite,  4MgO,  3CO2+ 
4H2O. 

-j-10H2O.  Sol.  in  considerable  amount  in 
H2C03+Aq  as  MgH2(CO3)2+Aq.  (Engel, 
C.  R.  100.  911.) 


Magnesium  carbonate,  MgCO3. 

A'i  hydrous.  Insol.  in  H2O.  1  1.  H2O  dis- 
solves 106  mg.  MgC03.  (Chevalet,  Z.  anal. 
8.91.)  Sol.  in  5071  pts.  H2O  at  15°.  (Krem- 
ers.)  MgCO3  combines  with  H2O  to  form 
MgCO3+3H2O,  and  +5H2O,  which  are  less 
sol.  in  H2O  than  anhydrous  salt.  (Engel, 
C.  R.  101.  814.) 

Very  hydroscopic.  About  20  g.  are  sol.  in 
1 1.  H2O.  (Engel,  C.  R.  1899,  129.  598.) 

0.7156  g.  are  sol.  in  1 1.  H2O  at  15°. 

0.627  g.  are  sol.  in  1  1.  H2O  at  15°  with 
vapour  pressure  of  CO2  equal  to  zero. 

6.977  grams  are  sol.  in  1 1.  H20  at  15°  with 
vapour  pressure  CO2  equal  to  1  atmos. 
(Treadwell  and  Reuter,  Z.  anorg.  1898,  17. 
202.) 

94.4  mg.  are  sol.  in  1  1.  of  CO2-free  water. 
(Gothe,  Ch.  Z.  1915,  39.  306.) 

Solubility  in  H2O  in  equilibrium  with 
Mg(HC03)2  and  CO2. 

Svstem:  MgCO3,  Mg(HC08)2  and  CO2  at 
30°  t). 


Total  Mg  (gram- 
atoms  per  liter) 

Mg  as  MgCOs 
Per  cent 

MgasMg(HCO3)2 
Per  cent 

0.00100 
0.00545 
0.00667 

50.00 
51.92 
53.93 

50.00 
48.08 
46.07 

Total  salts 
in  solution. 
Grams  per 
liter 

MgCOa 

Mg(HC03)2 

Grams 
per  liter 

Per  cent 

Grrms 
per  liter 

Per  cent 

0.1144 
0.6174 
0.7479 

0.0418 
0.2368 
0.3012 

36.5 
38.2 
40.3 

0.0726 
0.3806 
0.4467 

63.5 
61.7 
59.7 

Total  Mg 
(grams  per  liter) 

Mg  as  MgCOa 
(grams  per  liter) 

Mg  as 
Mg(HC03)2 
(grams  per  liter) 

0.02410 
0.13135 
0.16087 

0.01205 
0.06820 
0.08676 

0.01205 
0.06314 
0.07411 

Solubility   in   H2O     in    equilibrium  with 
Mg(HCO3)2  and  CO-2~Continued. 

System:  MgCO3,  Mg(HCO3)2  and  CO2   at 
30°  C. 


In  a  solution  near  the  saturation  point  and 
in  equilibrium  with  atmospheric  air  upwards 
of  50  per  cent  of  the  magnesium  is  in  the 
form  of  the  normal  carbonate.  When  the 
solution  is  brought  in  contact  with  the  solid 
phase,  the  proportion  of  the  base  combined 
as  normal  carbonate  falls  to  about  34  per 
cent,  or  lower.  (Cameron  and  Briggs,  J. 
phys.  Chem.  1901,  5.  552-3.) 

For  solubility  in  H2CO3+Aq,  see  Magne- 
sium hydrogen  carbonate. 

Scarcely  acted  upon  by  HCl+Aq.  (Senar- 
mont.) 

The  solubility  of  MgC03  in  NaCl+Aq 
when  in  contact  with  ordinary  air  •  increases 
with  increasing  concentration  of  NaCl  up 
to  a  maximum,  and  then  decreases.  (Cam- 
eron and  Seidell,  J.  phys.  Chem.  1903,  7.  579.) 


Solubility  of  MgC08  in  salts +Aq  in  equilib- 
rium with  an  atmosphere  free  from  CO2» 

NaCl+Aq;t  =  23°. 


Weight  of 
liter  of 
solution 

Grams 
NaCl  per 
liter 

Grams 
MgCOs 
per  liter 

Reacting 
weights 
NaCl 
per  liter 

Reacting 
weights 
MgCOa 
per  liter 

0.00210 
0.00500 
0.00630 
0.00699 
0.00650 
0.00550 
0.00470 
0.00350 

996.92 
1016.82 
1041.09 
1070.50 
1094.53 
1142.48 
1170.14 
1199.28 

0.0 
28.0 
59.5 
106.3 
147.4 
231.1 
272.9 
331.4 

0.176 
0.418 
0.527 
0.585 
0.544 
0.460 
0.393 
0.293 

0.000 
0.482 
1.025 
1.831 
2.539 
3.981 
4.701 
5.709 

(Cameron  and  Seidell,  J.  phys.  Chem.  1903,  7. 
585.) 

194 


CARBONATE,  MAGNESIUM 


Solubility  of  MgCO3  in  salts  +Aq  —  Continued 
Na2S04+Aq;t=24°. 

Solubility  in  salts  +Aq.  —  -Continued 

g.  salt  added  per  litre 

mg.MgCOs  dissolved 
per  litre 

Weight  of 
liter  of 
solution 

Grams 
Na2S04 
per  liter 

Grams 
MgCOs 
per  liter 

Reacting 
wts. 
Na2S04 
per  liter 

Reacting 
wts.  MgCO 
per  liter 

0.805g.  Na2SO4,  10H2O 
1.61  g. 
4.03g.            ,    " 

145.05 
162.05 
150.75 

997.52 
1021.24 
1047.60 
1080.95 
1133.85 
1157.34 
1206,03 
1223.91 
1241.99 

0.00 
25.12 
54.76 
95.68 
160.80 
191.90 
254.60 
278.50 
305.10 

0.216 
0.586 
0.828 
1.020 
1.230 
1.280 
1.338 
1.338 
1.388 

0.000 
0.178 
0.388 
0.678 
1.140 
1.360 
1.804 
1.973 
2.162 

0.00258 
0.00700 
0.00990 
0.01219 
0.01470 
0.01530 
0.01600 
0.01600 
0.01660 

0.53g.  Na2C03 
1.06g.       " 
2.65g.       " 

98.6 
53.5 
15.7 

0.51g.  MgCl2,  6H2O 
1.02g. 
2.55g. 

47.0 
39.5 
35.3 

The  solubility  of  MgCO3  in  CO2-free  water 
is  increased  by  the  addition  of  NaCl,  IS  aNO» 
or  Na2SO4,  10H2O  but  decreased  by  the  addi- 
tion of  Na2CO3  or  MgCl2,  6H20. 
(Gothe,  Ch.  Z.  1915,  39.  306.) 

Insol.  in  liquid  NH3.     (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 
Insol.  in  acetone.     (Naumann,   B.    1904, 
37.  4329.) 
Insol.  in  acetone  and  in  methylal.     (Eid- 
mann,  C.  C.  1899,  II.  1014.) 
Insol.   in   methyl   acetate   (Naumann,   B. 
1909,  42.  3790);  ethyl  acetate.     (Naumann, 
B.  1904,  37.  3601.) 
Min.    Magnesite.      Very   si.    attacked  by 
warm  cone.  HCl+Aq.    100  pts.  H2O  dissolve 
0.0027  pt.,  calculated  as  MgO.    (Lubavin.) 
Solution  in  H2O  contains  0.018  g.  Mg  and 
0.065  g.  C02  per  1.  at  20°.     (Wells,  J.  Am. 
Chem.  Soc.  1915,  37.  1705.) 
Solution  in  H2O  containing  27.2  g.  NaCl 
per  1.  contains  0.028  g.  Mg  and  0.086  g.  C02 
per  1.  at  20°.     (Wells,  J.  Am.  Chem.  Soc. 
1915,  37.  1705.) 
+H20. 
+2H2O.    Decomp.  by  suspension  in  H20 
into  basic  salt.    (Engel,  C.  R.  100.  911.) 
+3H20.    Small  quantities  of  this  salt  are 
wholly  dissolved  by  much  H2O.    (Bineau.) 
The  solution  contains  in  100  pts.  at  — 

0°       6.5°       8°        16° 
0.15  0.153  0.155  0.179  pts.  MgCO3-f3H20. 
(Norgaard,  1860.) 

Decomp.  by  boiling  H2O  into  a  basic  insol. 
salt  and  CO2.    100  pts.  H2O  dissolve  0.1518 
pt.  at  19°.    (Fritzsche,  Pogg.  37.  304.) 
Sol.  in  48  pts.  H20,  and  decomp.  by  large 
amt.    (Fourcroy.) 
100  pts.  H2O~  dissolve  0.1518  pt.  at  19°,  or 
sol.  in  658  pts.  H2O  at  19°.    (Beckurts,  J:  B. 
1881.  212.) 
100  pts.  H2O  dissolve  0.0812  pt.,  calculated 
as  MgO.    (Lubavin,  J.  russ.  Soc.  24.  389.) 
Solution  in  H2O  contains  0.36  g.  Mg  and 
1.01  g.  CO2  per  1.  at  20°.     (Wells,  J.  Am. 
Chem.  Soc.  1915,  37.  1707.) 
Solubility  in  H2O  sat.  with  C02  has  been 
determined  at  20°,  25°,  30°,  34°  and  39°  and 

t=35.5°. 

Weight  of 
liter  of 
solution 

Grams 
Na2S04 
per  liter 

Grams 
MgCOs 
per  liter 

Reacting 
weights 
Na2S04 
per  liter 

Reacting 
weights 
MgCOs 
per  liter 

995.15 
1032.89 
1067.23 
1094.77 
1120.38 
1151.70 
1179.82 
1196.32 
1236.52 

0.32 
41.84 
81.84 
116.56 
148.56 
186.70 
224.00 
247.20 
199.20 

0.131 
0.577 
0.753 
0.904 
0.962 
1.047 
1.088 
1.100 
1.130 

0^296 
0.579 
0.826 
1.052 
1.323 
1.587 
1.751 
2.120 

0.00156 
0.00689 
0.00900 
0.01080 
0.01149 
0.01251 
0.01300 
0.01314 
0.01350 

(Cameron  and  Seidell.) 
Na2CO3-fAq;t=25°. 

Weight  of 
liter  of 
solution 

Grams 
Na2COs 
per  liter 

Grams 
MgCOs 
per  liter 

Reacting 
weights 
Na2COs 
per  liter 

Reacting 
weights 
MgCOs 
per  liter 

096.84 
1019.89 
1047.72 
1082.47 
1118.91 
1147.66 
1166.05 
1189.38 

0.00 
23.12 
50.75 
86.42 
127.30 
160.80 
181.90 
213.20 

0.223 
0.288 
0.510 
0.879 
1.314 
1.636 
1.972 
2.317 

0.000 
0.220 
0.482 
0.820 
1.209 
1.526 
1.727 
2.024 

0.00266 
0.00344 
0.00620 
0.01027 
0.01570 
0.01955 
0.02357 
0.02770 

(Cameron  and  Seidell.) 
Solubility  in  salts  +Aq. 

g.  salt  added  per  litre 

mg.MgCOs  dissolved 
per  litre 

0.0 

94.4 

0.585g.  NaCl 
1.17g.       " 
2.93g.       " 

128.3 
134.4 
120.95 

0.85  g.  NaN03 
1.70g.       " 
4.25  g.       " 

122.85 
138.80 
137.20 

CARBONATE,  MAGNESIUM  HYDROGEN 


195 


at  CO2  pressures  corresponding  with  0.5  to 
30.3%  CO2  in  the  gas  phase.  (Leather  and 
Sen,  Chem.  Spc.  1915,  108  (2)  13.) 

Easily  sol.  in  acids,  even  when  dil 

Not  decomp.  by  1  pt.  H2SO4+6  pts.  al- 
cohol, or  by  alcoholic  solutions  of  glacial 
acetic,  racemir,  or  tartaric  acids,  but  is  slowly 
decomp.  by  alcoholic  solution  of  citric  acid, 
or  HN03+abs.  alcohol.  (Butini,  1827.) 

100  pts.  NaCl+Aq  (2.525%)  dissolve 
0.1250  pt.,  calculated  as  MgO.  (Lubavin.) 

1%  Na2CO3+Aq,  when  mixed  with  1% 
MgSO4+Aa,  cause  no  ppt.,  but  1.5-2%  solu- 
tions ppt.  this  salt.  (Brandes,  1825.) 

More  sol.  in  NH4Cl+Aq  than  CaC03.  Sol. 
in  NH4NO3+Aq,  but  less  easily  than  in 
NH4Cl+Aq. 

Solubility  in  KHCO3+Aq  at  t°. 
Values  are  given  in  mol./litre. 


t 

K 

Mg 

Solid  phase 

15° 

0.0 

0.0095 

MgC03+3H2O 

O.G992 

0.0131 

" 

0  .  1943 

0  0167 

" 

0  3992 

0.0211 

"      labile 

0.2681 

0.0192 

MgCOs  +3H20  +MgC03 

KHCOs  +4H2O 

0.5243 

0.0097 

MgC03,  KHCOs  +4H2O, 

0.6792 

0.0074 

" 

0:9810 

0.0028 

M 

25° 

0.0 

0.0087 

MgCOs+3H2O 

0.0985 

0.0115 

" 

0.2210 

0.014P 

" 

0.3188 

0.0175 

" 

0.3434 

0.0181 

" 

0.4216 

0.0205 

labile 

0.4985 

0.0207 

« 

0.3906 

C.0196 

MgCOs  +3H2O  +MgCOs 

KHC03+4H2O 

0.5893 

0.0128 

MgCOs,  KHC03-HH2O 

0.6406 

0.0117 

" 

0.788 

0.0089 

•« 

1.125 

0.0061 

" 

35° 

0.0 

0.0071 

MgCO3+3H2O 

0.1092 

0.0098 

" 

0.2001 

0.0132(?) 

•« 

0.2811 

0.0142 

«« 

0  3704 

0  0163 

<• 

0  4847 

0  0177 

« 

! 

0  5807 

G  0198 

" 

0  5088 

0  0184 

MgCO.3  +3H2O  +MgCO3) 

KHCOs  +4H2O 

• 

0  6231 

0  0153 

MgCOs,  KHCOs  +4H2O 

0  8435 

0  0119 

The  experiments  were  performed  in  such 
a  way  as  to  prevent,  as  far  as  possible,  loss  of 
CO2  from  the  solutions. 

f  (Auerbach,  Z.  Elektrochem.  1904,  10.  164.) 

1  1.  H2O,  containing  6%  MgSO4+7H2O  and 

a  little  NaCl,  dissolves  5  g.  MgCO3.  (Hunt, 
Sill.  Am.  J.  (2)  42.  49.) 

More  sol.  in  cold  alkali  borates+Aq  than 
in  hot.  (Wittstein.) 

Sol.  in  Na  citrate +Aq. 

+4H2O.    Efflorescent. 

+5H20.     Two  modifications. 

a.  Plates.  Sol.  in  600  pts.  H20  at  0-7°; 
solution  gradually  separates  out  MgCO3-f 
2H2O.  H2C03+Aq  sat.  at  3-4  atmos.  pres- 
sure dissolves  9%  at  0-4°,  MgSO4+Aq  dis- 
solves 4%  moist  salt  at  3-4°,  and  it  is 
easily  sol.  in  Na2CO3,  or  NaHCO3+Aq. 
(Norgaard.) 

13.  Prisms.  More  efflorescent  than  a.  Sol. 
in  600  pts.  H2O  but  not  in  MgSO4,  or  Na2CO3 
+Aq.  Both  forms  are  decomp.  by  boiling 
H2O.  (Norgaard.) 

Magnesium  hydrogen  carbonate, 

MgH2(C03)2(?). 

Known  only  in  solution. 

1  1.  H2CO3+Aq  sat.  at  1  atmos.  pressure 
dissolves  23.5  g.  MgCO3.  (Bineau.) 

1  1.  carbonic  acid  water  dissolves  0.115  g. 
magnesite  at  18°  and  0.75  m.  pressure. 
(Cossa,  B.  2.  697.) 

1  pt.  MgOO3  dissolves  in  H2O  saturated 
with  CO2  at  5°  and  a  pressure  of — 

123         456  atmospheres 
in  161    144   134   100.7   110   76  pts.  H2O 
(Merkel,  Techn.  J.  B.  1867.  213.) 

H2CO3+Aq  sat.  at  3-4  atmos.  pressure 
and  0-4°  dissolved  9%  MgCO3+5H2O. 
(Norgaard.) 

MgCO3+3H2O  is  sol.  in  72.4  pts.  H2CC3  + 
Aq  sat.  at  20°  and  ord.  pressure;  30.5  pts. 
H2CO3+Aq  sat.  at  2  atmos.  pfessure;  26.0 
pts.  H2CO3+Aq  sat.  at  3  atmos.  pressure; 
21.1  pts.  H2CO3+Aq  sat.  at  4  atmos.  pres- 
sure; 17.09  pts.  H2CO3-}-Aq  sat.  at  5  atmos. 
pressure.  (Beckurts,  J.  B.  1881.  212.) 

1.  H2O  sat.  with  CO2  at  p  pressure  and  t° 
dissolves  g.  MgC03. 


atmos. 


1.0 
2.1 
3.2 
4.7 
5.6 
6.2 
7.5 
9.0 


19.5 
19.5 
19.7 
19.0 
19.2 
19.2 
19.5 
18.7 


MggCOs 


.79 

.11 

.3 

.5 

.2 

.51 

.2 

.59 


P 

mm. 


751 
760 
762 
764 
764 
765 
765 
765 
765 


13.4 
19.5 
29.3 
46 
62 
70 
82 
91 
100 


MggCOs 


28.45 

25.79 

21.95 

15.7 

10.4 

8.1 

4.9 

2.4 

0.0 


(Engel  and  Ville,  C.  R.  93.  34.) 

The  low  figures  of  other  observers  are  due 
to  their  using  basic  carbonates.  By  very  care- 
ful experiments  it  was  found  that  1  1.  H2O 


196 


CARBONATE,  MAGNESIUM  POTASSIUM 


sat.  with  CO2  at  1  atmos.  pressure  and  t°  dis- 
solved the  following  amts.  of  MgC03: 


t° 

MgCO: 

t° 

MgCOs 

t° 

MgCOs 

3.5 
12 

35.6 
26.5 

18 
30 

22.1 
15.8 

40 
50 

22.1 
9.5 

(Engel,  G.  R,  100.  444.) 


Solubility  in  NaCl+Aq  at  23°C.  in  equilib- 
rium with  an  atmosphere  of  CO2. 

g.  NaCl  per  liter 

g.  Mg(HCO3)2per  liter 

7.0 
56.5 
119.7 
163.9 
224.8 
306.6 

30.64 
30.18 
-    27.88 
24.96 
20.78 
10.75 

(Cameron  and  Seidell,  ,T.  phys.  Chem.  1903, 


1.9540  g.  are  sol.  1  1.  H2O  at  15°.    (Tread- 

i.  ooz.; 

well  and  '  euter,  Z.  anorg.  1898,  17.  202.) 
MgH2(CO3)2  is  not  stable  except  in  the 
presence  of  free  C02. 

Solubility  in  Na2S04+Aq  at  23°  C.  in  equilib- 
rium with  an  atmosphere  of  CO2. 

At   15°  and  760  mm.,  a  solution  having 
the    partial   pressure    of    CO  2=0,    contains 

Strength  of  Na2SO4+Aq     g.  MgCHCOs)?  in  100  ccm. 

1.9540  g.  MgH2(C03)2  and  0.7156  g.  MgCO3 

0.0                                1.463 

per  liter.    (Treadwell  and  Ii  euter,  Z.  anorg. 

12%                             1.916 

1898,17.204.) 

saturated                           1  .  612 

(Cameron  ard  Seidell.) 

Solubility  of  MeH^COs)?  in  H2O  containing 
carbonic  acid,  at  15°.  . 

Magnesium  potassium  carbonate, 

MgK2(C03)2+4H20. 

a 

Quickly  decomp.  by  cold  H2O.     (Deville, 

•el 

0 

H 

g| 

a  u 

A.  ch.  (3)  33.  87.) 

-X   o3 

i  M 

8 

0*3  ^ 

'«"5 

M 

Ppt.    Decomp.  by  H2O.    (Reynolds,  Chem. 

•I  -si 

s  tc 

a> 

0"o.2 

Soc.  1898,  73,  264.) 

111 

~   S 

J 

S".2 

•H    gJ2 

M 

MgKH(CO3)2+4H20.    Insol.  in  H2O,  but 

fP 

•S  S 

•** 

tab 

So  ° 

.0  K 

S 

decomp.  thereby  into  an  insol.  basic  Mg  car- 

$$ 

c 

g 

MC 

g2 

bonate,  and  MgH2(CO3)2  and  KHCO3,  which 

S"* 

dissolve.    (Berzelius.) 

18.86 
5.47 
4.45 

143.3 
41.6 
33.8 

119.0 
86.6 
223.5 

1210.5 
1210.5 
1210.5 

.... 

201.6 
201.6 
201.6 

Magnesium  rubidium  hydrogen  carbonate, 
MgRbH(C03)2+4H20. 

1.54 

11.7 

1076.6 

77^3 

201^6 

Decomp.  in  the  air.     (Erdmann,  A.  1897, 

1.35 

10-3 

762.9 

76.5 

149.2 

294.  75.) 

1.0V 

8.2 

595  2 

80  7 

122  4 

0.62 

4.7 

366.3 

7o!i 

86^5 

Magnesium  sodium  carbonate,  MgCO3, 

0.60 

4.6 

341.7 

75.8 

78.8 

Na2CO8. 

0.33 

2.5 

.  .  . 

263.2 

74.8 

65.5 

Quickly  decomp.  with  H2O.     (Deville,  A, 

0.21 

1.6 

222.9 

77.1 

•  59.4 

ch.  (3)33.89.) 

0.14 

1.1 

216.9 

71.0 

56.6 

+15H20.    (Norgaard.) 

0.03 

0.3 

.  .  . 

203.6 

71  1 

54  5 

.  .  . 

203.3 

68.5 

53.6 

Magnesium  sodium  carbonate  'sodium  chlo- 

... 

196.0 

70.2 

52.9 

ride,  MgCO3,  Na2C03,  NaCl. 

203.6 

62.5 

52.0 

Decomp.  by  H2O.     (de  Schulten.  C.  R. 

195.4 

61.6 

51.1 

1896,  122.  1427.) 

•  •  • 

.  .  . 

•  •  • 

195.4 

64.1 

51.8 

(Treadwell  and  R  euter,  Z.  anorg.  1898,  17. 
200.) 


No  bicarbonate  of  magnesium  is  formed 
under  pressures  of  CO2  up  to  five  atmos- 
pheres at  0°.  (Cameron,  J .  phys.  Chem.  1908 
12.  570.) 

A  critical  analysis  and  recalculation  of 
results  of  Engel  and  others  is  given  fa 
Johnston  (J.  Am.  Chem.  Soc.  1915  37 


Permanent.  Practically  insol.  in  H20.  Sol. 
in  H2CO3+Aq  and  in  acids  generally. 

1 1.  H2O  dissolves  0. 065  g.  at  25°.  (Ageno 
and  Valla,  Att.  Accad.  Line.  1911, 20,  II.  706.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

Min.  Rhodochrosite. 

+  1A,  or  1H2O.  Insol.  in  H2O.  Sol.  in 
acids.  Sol.  in  H2CO3+Aq.  1  pt.  MnCO5 
requires  2000  pts.  H2COz+Aq  for  solution. 


CARBONATE,  POTASSIUM 


197 


(Lassaigne.)  Sol.  in  7680  pts.  H2O,  and  3840 
pts.  H2O  containing  CO2.  (Jahn.)  When 
freshly  precipitated  is  sol.  in  NH4  salts +Aq. 
(Wittstein.)  Not  more  sol.  in  H20  contain- 
ing Na2CO3  or  K2CO3  than  in  pure  H2O. 
(Ebelmen.)  Insol.  in  NH4C1,  or  NH4N03+ 
Aq.  (Brett.) 

Sol.  in  ferric  salts +Aq,  with  evolution  of 
CO2  and  pptn.  of  Fe2O6H6.  (Fuchs.) 

Not  pptd.  in  presence  of  Na  citrate. 
(Spiller.) 


Manganous  potassium  carbonate, 

MnK2(CO3)2+4H2O. 
Ppt.    Decomp.  by  H2O  alone. 
SI.  sol.  in  Mn(C2H3O2)2+Aq  or  K2CO3+ 
Aq.    (Reynolds,  Chem.  Soc.  1898,  73.  264.) 


Manganous  carbonate  hydroxylamine, 

4MnC03,  3NH30+2H20. 
Ppt.     Sol.   in   acids.      (Goldschmidt 
Syngros,  Z.  anorg.  5.  138.) 


and 


Mercurous  carbonate,  Hg2CO3. 

Ppt.  Decornp.  by  hot  H2O.  Sol.  in  hot  or 
warm  NH4Cl+Aq,  but  less  easily  than  mer- 
curic carbonate;  less  sol.  in  NH4NO3+Aq. 
(Brett,  1837.) 

SI.  sol.  in  K2CO3+Aq;  partially  sol.  with 
decomp.  in  NH4OH-f-Aq.  (Wittstein.) 


Mercuric  carbonate,  basic,  4HgO,  CO2. 

Can  be  washed  with  cold  H20  without  de- 
comp. (Millon,  A.  ch.  (3)  19.  368.) 

3HgO,  CO2.  Insol.  in  cold  H2O.  Sol.  in 
CC2-}-Aq;  si.  sol.  in  K2CO3+Aq.  Easily  sol. 
in  NH4Cl+Aq.  (Berzelius.) 


Neodymium  potassium  carbonate,  Nd2(C03)3, 

K2C03+12H2O. 

Ppt.     Sol.  in  30%  K2CO3+Aq.     (Meyer, 
Z.  anorg.  1904,  41.  105.) 


Neodymium  sodium  carbonate,  2Nd2(CO3)3, 
3Na2C03+22H2O(?). 

Ppt.    Easily  decomp. 

SI.  sol.  in  cone.  Na2CO3+Aq.  (Meyer,  Z. 
anorg.  1904,  41.  106.) 


Nickel  carbonate,  basic,  3NiO,  CO2+5H2O. 

Min.  Zaratile.    Easily  sol.  in  HCl+Aq. 

Pptd.  nickel  carbonate  is  a  basic  salt  of 
varying  composition.  Insol.  in  H20  or  H2C03 
+Ao.  Sol.  in  acids.  Sol.  in  (NH4)2CO3+Aq; 


very  si.  sol.  in  Na2CO3-fAq;  sol.  in  warm 
NH4Cl+Aq,  andKCN+Aq.    (Rose.) 

Not  pptd.  in  presence  of  Na  citrate.    (Spil- 
ler.) 


Nickel  carbonate,  NiCO3. 

1  1.  H,O  dissolves  0.0925  g  at  25%. 
(Ageno  and  Valla,  Att.  Accad.  Line.  1911, 
20,  II.  706.) 

Not  attacked  by  cold  cone.  HC1,  or  HNO, 
+Aq.  (Senarmont,  A.  ch.  (3)  30.  138.) 

+6H2O.  Sol.  in  acids.  (Deville,  A.  ch. 
(3)  35.  446.) 

See  also  Carbonate,  nickel,  basic. 


Nickel  potassium  carbonate,  NiCO3,  K2CO3-f- 

4H20. 

Ppt.    (Deville,  A.  ch.  (3)  33.  96.) 
NiC03,KHC03+4H20.   Decomp.  by  H2O, 

but  may  be  washed  by  KHCO3+Aq  without 

decomp.    (Rose,  Pogg.  84.  566.) 


Nickel  sodium  carbonate,  NiC03,  Na2CO8+ 

10H2O. 
Ppt.    (Deville.) 

Nickel  carbonate  hydroxylamine,  2Ni(OH)2, 
4NiC03,  5NH2OH+7H2O. 

Ppt.  (Goldschmidt  and  Syngros,  Z.  anorg. 
1894,  5.  143.) 

2Ni(OH)2,  4NiCO3,  6NH2OH+6H2O. 

Ppt.    (Goldschmidt  and  Syngros.) 


Palladious    carbonate,    PdCO3,    9PdO  + 

10H2O. 

Insol.  in  H2O;  partly  sol.  in  NH4OH+Aq; 
si.  sol.  in  Na2CO3+Aq;  sol.  in  acids.  (Kane, 
1842.) 

Potassium  carbonate,  K2CO3. 

Deliquescent.  Very  sol.  in  H2O  with  evolu- 
tion of  heat. 

Sol.  in  1.05  pts.  H2O  at  3°;  0.962  pt.  at  6°;  0.900 
pt.  at  12.6°;  0.747  pt.  at  26°;  and  0.490  pt.  at  70°. 
(Osann.) 

Sol.  in  0.92  pt.  H2O.    (M.  R.  and  P.) 

Sol.  in  0.922  pt.  H2O  at  15°.     (Gerlach.) 

Sol.  in  1  pt.  H2O.     (Abl.) 

100  pts.  H2O  at  15.5°  dissolve  100  pts.  K2CO3.  (lire's 
Diet.) 


Solubility  in  100  pt?.  H2O  at  t°. 


t° 

Pts. 
K2C03 

t° 

40 
50 
60 
70 

Pts. 
K2C03 

t° 

Pts. 
K2C03 

0 
10 

20 
30 

83.12 

88.72 
94.06 
100.09 

106.20 
112.90 
119.24 
127.10 

80 
90 
100 
135 

134.25 
143  18 
153.66 
205.11 

(Poggiale,  A.  ch.  (3)  8.  468.) 

CARBONATE,  POTASSIUM 


Solubility  in  100  pts.  H20  at  t°. 

Sp.  gr.  of  K2CO3+Aq  at  15°  —  Continued. 

t° 

0 
1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
34 
35 
36 
37 
38 
39 
40 
41 
42 
43 
44 
45 

Pts. 
K2C03 

t° 

Pts. 
K2C03 

t° 

Pts. 
K2C03 

%  K2C03 

Sp.  gr. 

%  K2C03 

Sp.  gr. 

23.496 
24.475 
25.454 
26.432 
27.412 
28.391 
29  .  360 
30.349 
31.328 
32.807 

1.2836 
1  .  2980 
1  3078 
1.3177 
1  .  3277 
1.3378 
1  .  3480 
1  .  3585 
1  .  3692 
1.3803 

33.286 
34  .  265 
35  .  244 
36  .  223 
37  .  202 
38.181 
39.160 
40.139 
40  .  504 

1.8915 

1  .  4030 
.4147 
.  4265 
.4384 
.4504 
.  4620 
.4750 
.4812 

89.4 

94 
97 
100 
102 
104 
105 
106 
107 
108 
109 
109 
109 
110 
110 
110 
111 
111 
111 
111 
112 
112 
112 
112 
112 
113 
113 
113 
113 
114 
114 
114 
114 
115 
115 
115 
115 
116 
116 
116 
117 
117 
117 
118 
118 
119 

46 
47 
48 
49 
50 
51 
52 
53 
54 
55 
56 
57 
58 
59 
60 
61 
62 
63 
64 
65 
66 
67 
68 
69 
70 
71 
72 
73 
74 
75 
76 
77 
78 
79 
80 
81 
82 
83 
84 
85 
86 
87 
88 
89 
90 

119 
120 
120 
121 
121 
122 
122 
123 
124 
124 
125 
125 
126 
127 
127 
128 
128 
129 
130 
130 
131 
132 
132 
133 
133 
134 
135 
135 
136 
137 
137 
138 
139 
139 
140 
141 
141 
142 
143 
144 
144 
145 
146 
147 
147 

91 
92 
93 
94 
95 
96 
97 
98 
99 
100 
101 
102 
103 
104 
105 
106 
107 
108 
109 
110 
111 
112 
113 
114 
115 
116 
117 
118 
119 
120 
121 
122 
123 
124 
125 
126 
127 
128 
129 
130 
131 
132 
133 
134 
135 

148 
149 
150 
151 
151 
152 
153 
154 
155 
156 
157 
158 
159 
160 
161 
162 
163 
164 
166 
167 
168 
169 
171 
172 
173 
175 
176 
178 
179 
181 
182 
184 
185 
187 
188 
190 
191 
193 
195 
196 
198 
200 
201 
203 
205 

Sp.gr 

(Tiinnerman.) 
.  and  boiling-point  of  K2COs+Aq. 

K2C03 

Sp.   gr. 

B.-pt. 

KzCOa 

Sp.   gr. 

B.-pt. 

4.7 
9.0 
13.2 
16.8 
20.5 
24.0 
27.3 
30.5 
33.6 
36.2 
39.0 
41.7 

1.06 
1.11 
1.15 
1.19 
1.22 
1.25 
1.28 
1.31 
1.34 
1.38 
1.41 
1.44 

100.56° 
100.56 
101.11 
101.11 
101.66 
102.22 
102.78 
103,33 
104.44 
105.56 
107.22 
108  .  33 

43.3 
45.8 
48.8 
52.1 
56.0 
60.4 
65.5 
71.8 
79.2 
88.4 
100.0 

1.46 
1.50 
1/54 
1.58 
1.63 
1.70 
1.80 
1.95 
2.15 
2.40 
2.60 

109.44° 
111.11 
112.78 
114.44 
116.11 
117.78 
119.44 
122  22 
125  .  5<i 
129.44 
137.78 

Sp. 

(Dalton.) 

gr.  of  K2CO3+Aq  at  17.5C. 

K2C03 

Sp.  gr. 

K2CO3 

19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
34 
35 

Sp.  gr. 

K2C03 

Sp.  gr. 

1 

2 
3 
4 

7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 

1.009 
1.018 
.027 
.036 
.045 
.054 
.064 
073 
.082 
.092 
.102 
.112 
.122 
.132 
.141 
.151 
.161 
1.172 

1.182 
1.192 
1.203 
1.213 
1.224 
1.235 
1.245 
1.256 
1.267 
1.278 
1.289 
1.3CO 
1.312 
1.323 
1.334 
1.345 
1.357 

36 
37 
38 
39 
40 
41 
42 
43 
44 
45 
46 
47 
48 
49 
5C 
51 
52 

.368 
.380 
.392 
.404 
.416 
.429 
.441 
.453 
1.466 
1.478 
1.489 
1.503 
1.516 
0.529 
1.542 
1.555 
1.569 

(Mulder,  Sc  eik.  Verhandel.  1864.  97.) 
112  g.  are  sol.  in  100  g.  H2O  at  20°.    (Frank- 
forter,  J.  Am.  Chem.  Soc.  1914,  36.  1106.) 

Sp.  gr.  of  K2CO3+Aq  at  15°. 

(Hager,  Comm.  1883.) 

The  sp.gr.  increases  or  diminishes  between 
8°  and  20°  by  a  decrease  or  increase  of  temp, 
of  1°  by  the  following  amounts:— 

%  K2C03 

Sp.  gr. 

%  K2COs 

Sp.  gr. 

0.489 
0.979 
1.958 
2.934 
3.916 
4.895 
5  .  874 
6.853 
7.832 
8.811 
9.790 
10.769 

1.0048 
.0098 
.0108 
.0299 
.0401 
.0505 
.0611 
1.0719 
1  .  0829 
1  .  0940 
1  .  1052 
1.1166 

11.748 
12  .  727 
13.706 
14  .  685 
15.664 
16.643 
17.622 
18.601 
19.580 
20.539 
21.538 
22.517 

1  .  1282 
1  .  1400 
1  .  1520 
1  .  1642 
1  .  1766 
1  .  1892 
1.2020 
1.2150 
1  .  2282 
1.2417 
1.2554 
1.2694 

%  K2COs 

Corr. 

40-50 
30--40 
20-30 
10-20 

0.0007 
0.0005 
0.0003 
O.OOC2 

(Hager.) 

CARBONATE,  POTASSIUM 


199 


Sp.  gr.  of  K2CO3+Aq  at  15°. 

B.-pt.  of  K2CO,+Aq  containing  pts.  K2CO8 

to  100  pts.  H20.    G=  according  to  Ger- 
lach (Z.  anal.  26.  459);  L  =  according  to 

%  K2C03 

Sp.  gr. 

%  K2C03 

Sp.  gr. 

1 

1  00914 

28 

1   27RQ^ 

Legrand  (A.  ch.  (2)  69.  438). 

2 

1.01829 

29 

1.28999 

B.-pt 

G 

L 

3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 

1  .  02743 
1.03658 
1.04572 
1.05513 
1.06354 
1.07396 
1.08337 
1.09278 
1  .  10258 
1.11238 
1.12219 
1.13199 
1.14179 
1.15200 

30 
31 
32 
33 
34 
35 
36 
37 
38 
39 
40 
41 
42 
43 

1.30105 
1.31261 
1  32417 
1.33573 
1.34729 
1.35885 
1.37082 
1.38279 
1.39476 
1.40673 
1.41870 
1.43104 
1.44388 
1.44573 

101° 
102 
103 
104 
105 
106 
107 
108 
109 
110 
111 
112 
113 
114 

11.5 
22.5 
32 
40 
47.5 
54.5 
61 
67 
73 
78.5 
83.5 
88.5 
93.5 
qc  £ 

13 
22.5 
31 
38.8 
46.1 
53.1 
59.6 
65.9 
71.9 
77.6 
83.0 
88.2 
93.2 

GO    A 

17 
18 
19 
20 
21 
22 
23 
24 
25 
26 

1.16222 
1.17243 
1  .  18265 
1.19286 
1.20344 
1.21402 
1.22459 
1.23517 
1.24575 
1.25681 

44 
45 
46 
47 
48 
49 
50 
51 
52 
52.024 

1.46807 
1.48041 
1.49314 
1.50588 
.51861 
.53135 
.54408 
.55728 
.57048 
.57079 

115 
116 
117 
118 
119 
120 
121 
122 
123 
124 

103.5 
108.5 
113.5 
117.5 
122.5 
127.5 
.    132.5 
137.5 
142.5 
147.5 

102.8 
107.5 
112.3 
117.1 
122.0 
127.0 
132.0 
137.0 
142.0 
147.1 

27 

1  .  26787 

125 

152.5 

152.2 

(Gerlach,  Z.  anal.  8.  279.) 

126 
127 

158 
163.5 

157.3 
162.5 

128 

169.5 

167.7 

129 

175  5 

172  9 

Sp.  gr.  of  K2CO3-f  Aq  at  15°. 

130 

181.5 

1  017   c 

178.1 

1  OO      A 

%  K2C03           Sp.  gr. 

%  K2CO3 

Sp.  gr. 

132 

193.5 

loo.* 

188.8 

5             1.0449 
10            1.0919 
20             1.1920 

30 
40 
50 

1.3002 
1.4170 
1.5428 

133 
133.3 
134 
135 

199.5 
202.5 

194.2 

199!  6 
205.0 

(Kohlrausch,  W.  Ann.  1879.  1.) 

K2C03+Aq  containing  10%  K2COS  boils  at 

100.8° 
K2CO8+Aq  containing  20%  K2CO3  boils  at 

102.2° 
K2CO3+Aq  containing  30%  K2CO3  boils  at 

104.5C 
K2CO3+Aq  containing  40%  K2CO3  boils  at 

108.6° 
K2CO3+Aq  containing  50%  K2CO3  boils  at 

115.2° 

(Gerlach.) 


Sat.  K2C03+Aq  containing  158  pts.  K2CO, 
to  100  pts.  H2O  forms  a  crust  at  126°;  highest 
temp,  observed  134.9°.  (Gerlach,  Z.  anal.  £ 
427.) 


When  K2CO3+Aq  is  sat.  with  NH8,  two 
ayers  form.  When  K2Cp8  is  added  to 
^H4OH+Aq,  it  dissolves  with  formation  of 
;wo  layers  and  evolution  of  NH8.  The  same 
;akes  place  also  when  sat.  KiCO3+Aq  and 
NH4OH+Aq  are  brought  together;  (Girard, 
Bull.  Soc.  (2)  43.  552.) 
olubility  of  K2C03+KHC03  in  H2O  at~0°. 


g.  per  100  cc.  solution 

Sp.  gr. 

K2C03 

KHCOs 

0.0 

21.2 

1.133 

11.8 

15.3 

1.182 

16.7 

12.6 

1.200 

23.8 

10.3 

1.241 

34.0 

7.6 

1.298 

43.0 

5.9 

1.350 

51.6 

4.9 

1.398 

60.5 

3.8 

1.448 

81.4          1 

0.0 

1.542 

(Engel,  A.  ch.  1888,  (6)  13.  348.) 

200 


CARBONATE,  POTASSIUM 


Equilibrium  between  K2CO3  and  KHCO3  in 
H2O  and  in  contact  with  the  air.  Sys- 
tem: K2C03,  KHC03,  and  C02  at  25°  c. 


Grams 
atoms  K 
per  liter 

Amount  of 
solution 
used  for 
titration 
cc. 

Amount  K 
combined 
as  K2CO3 
Per  cent 

Amount  K 
combined 
as  KHCOs 
Per  cent 

0.393 

5 

77.5 

22.5 

5 

0.553 

2 

83.9 

16.1 

5 

1.025 

2 

86.8 

13.2 

2 

2 

1.865 

2 

91.4 

8.6 

2 

2.820 

2 

89.0 

11.0 

2 

3.710 

2 

88.6 

11.4 

2 

4.310 

1 

89.6 

10.4 

1 

5.695 

1 

88.7 

11.3 

1 

(Cameron  and  B 


J.  phys.  Chem.  1901, 
546.) 


Solubility  of  K2C03+Na2C03  in  H2O  at 

25°. 


g.  per  100  g. 

g.  per  100  g 

solution 

H2O 

N 

O 

« 

6 

Solid  phase 

8 

i 

5 

M 

1 

£ 

1 

52.82 

0 

112 

0 

K2CO3.2H2O 

52.0 

1.0 

110.7 

2.2 

«« 

50.7 

2.6 

108.7 

5.7 

" 

49.0 

4.6 

105.5 

10.0 

K2C03.2H2O  +Na2C03, 

* 

K2CO3.12H2O 

46.5 

46.2 

4.3 
5.2 

94.6 
94.8 

8.8 
10.6 

Na2C03>  K2CO3.12H20 

41.0 

6.3 

77.6 

11.8 

37.7 

7.0 

68.3 

12.6 

31.0 

10.5 

53.0 

17.9 

29.8 

11.3 

50.5 

19.1 

25.2 

14.1 

41.4 

23.2 

22.4 

16.6 

36.8 

27.3 

19.8 

18.7 

32.1 

30.3 

19.1 

19.7 

31.2 

32.1 

15.1 

23.2 

24.5 

37.6 

Na2CO3,  K2CO3.12H2O 

14.5 

22.8 

23.1 

36.4 

+Na2CO3.10H2O 
Na2CO3  10H2O 

10.8 

22.7 

16.2 

34.0 

10.7 

22.4 

16.0 

33.5 

4.7 

21.9 

6.4 

29.8 

0 

22.71 

0 

29.37 

(Osaka,  J.  Tok.  Chem.  Soc.  1911,  32.  870.) 


Solubility  of  K2CO3+Na2CO3  in  H2O  at  24.2°. 


In  1000  ccm.  H2O 


Na2CO3        K2COs 


28.35 
354.2 
369.7 
363.0 
330.8 
273.8 
187.2 
130.0 
137  9 
112.3 

95.2 
25.5 


150.03 
226.6 
243.5 
282.7 
344.9 
483.9 
921  5 
982  6 
1074.0 

1085.1 
1108.6 
1125.7 


Solid  phase 


Na2CO3 
Na2CO3,  K2CO3.6H2O 


Na2C03,  K2C03.6H20  + 

Na2CO3 
d 

K2C03 


(Kremann  and  Zitek,  M.  1909,  30.  317.) 


Solubility  of  K2CO3+Na2CO3  in  H2O  at  10C 


In  1000  ccm.  H2O 


Na2C03       K2C03 


119.8 
176.4 
108. 
61.19 


354.1 

500.1 

0052.9 

1084.0 


Solid  phase 


Na2C03 

« 


Na2CO3,  K2CO3 
K2COS 


(Kremann  and  Zitek,  M.  1909,  30.  324.) 


Solubility  of  K2CO3+KNO8  in  H2O  at  25.2C 


1  1.  of  the  solution  contains 


Mol.  K2C03 

Mol.  KNOa 

0.00 
0.59 
1.35 
2.10 
2.70 
3.58 

3.217 
2.62 
1.97 
1.46 
1.14 
0.79 

(Touren,  C.  R.  1900,  131.  259.) 


Solubility  of  K2CO3+KNO3  in  H2O  at  10°. 


In  1000  ccm.  H2O 

Solid  phrase 

,    KNOa 

K2C03 

208.9 
26.62 

1076  !o 
1084.0 

KNO3 
KN03,  K2C08 
K2C03 

(Kremann  and  Zitek,  M.  1909,  30.  325.) 


CARBONATE,  POTASSIUM 


201 


Solubility  of  K2CO3+KNO3  in  H2O  at  24.2° 


In  1000  ccm.  H2O 


KNOa 


376.85 

285.00 

161.67 

141.80 

73.04 

38.78 

31.11 


K2C03 


130.3 
348.4 
371.9 
688.1 
878.3 
1112.2 


Solid  phase 


KNO? 


KN03,  K2C03 


(Kremann  and  Zitek,  M.  1909,  30.  316.) 
Solubility  of  K2CO3+KC1  in  H2O  at  30°. 


KoCOs 

ft 

Solid  phase 

53.27 
52.22 
51.66 

0 
1.03 
1.07 

K2C03.l^H2b+KCl 
KC1 

1.64 
0 

26*22 
28.01 

KC1 

u 

*  Author  gives  intermediary  data, 
(de  Waal,  Dissert.  1910.) 
Solubility  of  K2CO3+KQH  in  H2O  at  20°. 

%  KOH  %  K2C03  Solid  phase 


55.75 
55.14 

53.77 

* 

0 


0 

2.05 
2.50 

53*27 


KOH.2H2O 
KOH.2H2O+K2CO3.13/6H2O 


K2C03.1^H20 


*  Author  gives  intermediary  data, 
(de  Waal,  Dissert.  1910.) 

Insol.  in  liquid  NH3.     (Franklin,  Am.  Ch. 
J.  1898,  20,  828.) 

Sol.  in  9  pts.  alcohol  of  17°  B.    Insol.  in 
absolute  alcohol. 

Not  decomp.  by  1  pt.  H2SO4+6  pts.  ab- 
solute alcohol.    Not  decomp.  by  1  pt.  HNO3+ 
6  pts.  absolute  alcohol.    Not  decomp.  by  an 
alcoholic  solution  of  HC1,  oxalic,  racemic,  tar- 
taric,  or  glacial  acetic  acids,  but  is  decomp.  by 
alcoholic  solution  of  citric  acid. 
Solubility  in  methyl  alcohol.    Composition  of 
liquids  in  equilibrium  with  solid  K2CO3 
att°. 


t° 

-30 
-20 
-20 
0 
0 
+17 
35 

Upper  layer 

Lower  layer 

8 

M 
£ 

K 
C 

te 
o 

k? 

Q 
a 
ss 

§ 

$ 

g 
o 
£ 

Q 

W 

£* 

21.7 
13.8 
12.4 
7.6 
7.4 
6.2 
5.0 

42.2 
52.1 

36.1 
34.1 



44.2 
46.3 
46.6 
48.3 

8.2 
6.7 
6.6 
5.7 
4.3 

47.6 
47 
46.8 
46 
44.7 

66.3 

26.1 

69.6 
72.  P 

24.2 
22.1 

(de  Bruyn,  Z.  phys.  Ch.  1900,  32.  63  and  ff.) 


Solubility  in  ethyl  alcohol.  Composition  of 
liquids  in  equilibrium  with  solid  K2CO3 
at  t°. 


t° 

Upper  layer 

Lower  layer 

8 

« 

&s 

w 

c 
B 
d 
SS 

g 

t£ 

K 
£ 

6 
tf? 

o 
5$ 

-18 
0 
+17 
35 
50 
75 

0.03 
0.04 
0.06 
0.07 
0.09 
0.12 

90.3 
91.9 
91.5 
90.9 
91.8 
91.4 

9.7 
8.1 
8.4 
9 
8.1 
8.5 

51.2 
51.3 
52.1 
53  4 
55.3 
57.9 

0.2 
0.2 
0.2 
0.2 
0.2 
2.0 

48.6 
48.5 
47.7 
46.4 
44.5 
40.9 

(de  Bruyn.) 

Solubility  in  ethyl  alcohol  +Aq  at  25°. 
When  K2CO3  is  dissolved  in  ethyl  alcohol + 
Aq  two  layers  are  formed,  the  compositions  of 
which  are  as  follows: 


Upper  layer 


ale 


81.25 
71.67 
56.98 
53.92 
50.21 
43.93 
37.64 
28.43 


H2O       K2CO3 


18.61 
27.91 
41.55 
44.13 
47.24 
52.04 
56.45 
61.57 


0.14 
0.42 
1.47 
2.05 
2.55 
3.92 
5.90 
10.00 


Lower  layer 


%  %  70 

alcohol        H20       K2C0.3 


0.82 

1.79 

4.02 

4.88 

5.54 

7.71 

10.54 

15.73 


42 
61 
73 
87 
06 
56 
40 
38 


43.76 
36.60 
30.25 
28.25 
27.41 
24.74 
22.06 
17.90 


(Cuno,  W.  Ann.  1909,  (4)  28.  664.) 
Solubility  of  K2CO3  in  alcohol +Aq  at  30C 


53.27 
53.09 


0.13 


0.04 


Alco°hol 


0 
0.1 


90.49 


99.92 


46.73 
46.81 


9.38 


0.04 


Solid  phase 


K2C03.1^H20 


K2C03 


K2CO,+K2CO3. 


*  Solution  separates  into  two  layers, 
(de  Waal,  Dissert.  Leiden,  1910.) 

A  full  discussion  ot  the  solubility  of  K2COS 
in  methyl,  ethyl,  propyl,  isopropyl,  and  allyl 
alcohols  is  given  by  Frankforter  and  Frary 
(J.  phys.  Ch.  1913,  17.  402),  and  Frankforter 
and  Temple  (J.  Am.  Chem.  Soc.  1915,  37. 
2697). 


202 


CARBONATE,  POTASSIUM  HYDROGEN 


K2CO3  will  "salt  out"  acetone  from  aqueous 
solution.  The  table  shows  the  composi- 
tion of  the  solutions  at  the  points  at 
which  inhomogeneous  solutions  of  K2CO3, 
acetone  and  H2O  just  become  homoge- 
neous at  20°.  100  g.  of  the  solution  con- 
tain: 


K2C03 

H*b 

g. 

acetone 

K2C03 

Hg;0 

g. 

acetone 

18.84 

73.22 

7.94 

2.43 

55.36 

42.21 

13.32 

71.38 

15.30 

22.29 

72.81 

4.90 

11.83 

70.34 

17.83 

17.86 

73.12 

9.02 

10.13 

69.03 

20.84 

15.81 

72.53 

11.66 

8.24 

67.31 

24.45 

14.39 

71.89 

13.72 

7.22 

65.99 

26.79 

10.29 

69.46 

20.25 

6.04 

64.39 

29.57 

1.91 

54.05 

44.04 

28.87 

69.08 

2  05 

1.76 

52.86 

45.38 

23.94 

71.98 

4  08 

1.60 

51.60 

46.80 

21.52 

72.75 

5.33 

1.29 

49.57 

49.14 

19.60 

73.10 

7.70 

1.08 

47.86 

51.06 

6.46 

65.34 

28.20 

0.94 

46.73 

52.33 

5.91 

64.65 

29.44 

0.75 

44.72 

54.53 

5.60 

63.93 

30.47 

0.66 

43.31 

56.03 

5.04 

62.80 

32.16 

0.60 

42.49 

56.91 

4.50 

61.48 

34.02 

0.54 

41.73 

57.73 

3.80 

59.79 

36.41 

0.50 

40.69 

58.81 

3.18 

57.95 

38.87 

0.46 

40.48 

60.06 

2.73 

56.50 

40.77 

(Frankforter  and  Cohen,  J.  Am.  Chem.  Soc. 
1914,  36.  1121.) 

Insol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1370.) 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,  34.  314.)  . 

Sol.  in  phenol. 

Sol.  in  13.5  pts.  glycerine  of  1.225  sp.  gr. 
(Vogel,N.Repert.  16.557.) 

100  g.  sat.  K2CO3+  sugar  +Aq  contains 
22.44  g.  K2CO3  and  56  g.  sugar  at  31.25° 
(Kohler,  Z.  Ver.  Zuckerind.  1897,  47.  447.) 


Very  deliquescent.     (Pohl.) 

Deliquescent  only  in  very  moist  air. 
(Stadeler.) 

Sol.  in  H2O  with  evolution  of  heat.    (Pohl.) 

Sol.  at  17.6°  with  absorption  of  heat,  at  32° 
with  evolution  of  heat,  and  at  25°  with  neither 
absorption  nor  evolution  of  heat.  (Berthelot, 
C.  R.  78.  1722.) 

Sat.  solution  of  K2C03+1^H2O  in  H2O 
contains  53.27  g.  anhydrous  K2CO3  in  100  g. 
solution  at  30°.  (de  Waal,  Dissert.  1910.) 

+2H2O.  Salt  usually  given  as  containing 
1^H2O  contains  2H20.  (Gerlach,  Z.  anal. 
26.  460.) 

Sat.  solution  of  K2CO3+2H2O  contains 
112  g.  anhydrous  K2COi  in  100  g.  H2O  at  25°. 
(Osaka,  J.  Tok.  Ch.  Soc.  1911,  32/870.) 

-f  4H2O.  Not  deliquescent  in  closed  vessels. 
(Gerlach,  I.  c.) 

Potassium  hydrogen  carbonate,  KHCO3. 
Not  deliquescent. 


Sol.  in  3.5  pts.  H2O  at  15°.  (Redwood.)  Sol.  in  4 
pts.  H2O  at  moderate  temperatures.  (Bergmann.)  Sol. 
in  0.8333  pt.  boiling  H2O  (Pelletier) ;  in  4  pts.  cold,  and 
1.2  pts.  boiling  H2O  (M.  R.  and  P.'s  Pharm.).  Sol.  in 
4  pts.  H2O  at  18.75°.  (Abl.)  100  pts.  H2O  at  15.5° 
dissolve  30  pts.  and  at  100°,  83  pts.  (Ure's  Diet.) 

100  pts.  H2O  at  10-11.2°  dissolve  26.1  pts.  KHCOs, 
and  the  sp.  gr.  of  solution  is  1.1536.  (Anthon,  Dingl. 
161.  216.) 

100  pts.  H2O  dissolve  at— 
0°         10°        20°       30° 
19.61     23.23    26.91    30.57  pts.  KHCO,, 
40°        50°        60°        70° 
34.15    37.92    41.35    45.24  pts.  KHCO3. 
(Poggiale,  A.  ch.  (3)  8.  468.) 

100  pts.  H2O  dissolve  pts.  KHCO3  at  t°. 


t° 

Pts.  KHCOs 

t° 

Pts.  KHCOs 

0 
20 

22.4 
33.2 

40 
60 

45.2 
46.4 

(Dibbits,  J.  pr.  (2)  10.  417.) 

Sp.  gr.  of  KHCO3+Aq  at  15°  containing 
5%  KHCO3  =  1.0328;  containing  10%  KHCO3 
=  1.0674.  (Kohlrausch,  Z.  anal.  28.  472.) 

Sol.  in  12CO  pts.  boiling  alcohol.  (Berthol- 
let.)  Insol.  in  alcohol.  (Dumas.) 

100  pts.  H2O  dissolve  19.3  pts.  KHCO3  and 
8.3  pts.  NaHC03  if  the  sat.  solution  of  latter 
is  sat.  with  former;  and  26.1  pts.  KHCO3  and 
6.0  pts.  NaHCO3,  if  the  sat.  solution  of  the 
former  is  sat.  with  the  latter,  all  at  10°. 
(Mulder,  J.  B.  1866.  67.) 

Insol.  in  sat.  K2CO3+Aq.  (Engel,  C.  R. 
102.  365.) 

Solubility  of  KHCO3+KNO3  in  H2O  in  an 
atmosphere  of  CO2. 


1  litre  of  the  solution  contains 

at  14.5° 

at  25.2° 

Mol.  KHCOs 

Mol.  KNC)3 

Mol.  KHCOt 

Mol.  KNOs 

0.00 

2.33 

0.00 

3.28 

0.39 

2.17 

0.89 

2.84 

0.76 

2.03 

1.33 

2.65 

1.16 

1.92 

1.91 

2.45 

1.55 

1.81 

This  case  is  complicated  by  the  fact  that 
KN03  is  more  sol.  in  H2O  sat.  with  CO2  than 
in  pure  H2O. 

(Touren,  C.  R.  1900,  131.  261.) 

Insol.  in  benzonitrile  (Naumann,  B.  1914, 
47.  1370.) 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  "ethyl  acetate  (Naumann, 
B.  1Q10,  43.  314.) 

Potassium  praseodymium  carbonate,  K2CO3, 

Pr2(CO3)3-}-12H2O. 

Ppt.  Sol.  in  30%  K2CO3+Aq.  (Meyer,  Z. 
anorg.  1904,  41.  104.) 


CARBONATE,  SODIUM 


203 


Potassium     samarium     carbonate,     K2CO3, 

Sm2(CO8)3  +  12H2O. 
(Cleve.) 

Potassium  silver  carbonate,  KAgCO3. 

Decomp.  by  H2O.  (de  Schulten,  C.  R. 
105.  811.) 

Ppt.  Decomp.  by  H2O.  (Reynolds,  Chem. 
Soc.  1898,  73.  265.) 

Potassium  sodium  carbonate,  KNaCO3  + 
6H2O. 

Slightly  efflorescent.  Sol.  in  0.75  pt.  H2O 
at  12.5°;  in  0.54  pt.  H2O  at  15°. 

Sat.  solution  at  15°  has  sp.  gr.  =  1.366. 
(Stolba,  J.  pr.  94.  406.) 

Decomp.  by  recrystallizing  from  H2O,  but 
crystallizes  undecomposed  from  sat.  K2CO3+ 
Aq. 

Sol.  in  H2O.     (Osaka,  C.  A.  1911.  2601.) 

See  K2CO3+Na2CO3  under  Na2CO3. 

+3H2O.  (Kremann  and  Zitek,  M.  1909. 
30.  317.)  Does  not  exist.  (Osaka.) 

K2CO3,  2Na2CO3  +  18H2O.  SI.  efflorescent. 
Very  sol.  in  H2O.  (Marignac.) 

Potassium   stannous   carbonate,   K2CO3, 

2SnCO3+2H2O. 
Decomp.  by  H2O.    (DeviUe.) 

Potassium    uranyl    carbonate,    2K2CO:, 
(UO2)CO3. 

Sol.  without  decomp.  in  13.5  pts.  H2O  at 
15°,  and  in  somewhat  less  warm  H2O.  Sol. 
in  boiling  H2O  with  decomp. 

More  sol.  in  K2CO3,  or  KHCOc+Aq  than 
in  H2O.  (Rose.) 

Insol.  in  alcohol.  (Ebelmen,  A.  ch.  (3)  5. 
189.) 

Potassium    zinc    carbonate,    4K2O,    6ZnO, 

11CO2+8H2O. 

Can  be  washed  with  cold  H2O  without 
decomp.  (Deville,  A.  ch.  (3)  33.  99.) 

Praseodymium  carbonate,  Pr2(COc)3+8H2O. 
Sol.  in  H2O.     (von  Schule,  Z.  anorg.  1898, 
18.  362.) 

Praseodymium  sodium  carbonate, 

2Pr2(CO3)3,  3Na2CO3+22H2O(?). 
Ppt.     Easily  decomp.     (Meyer,  Z.  anorg. 
1904,  41.  105.) 

Radium  carbonate. 

Less  sol.  in  H2O  than  corresponding  Ba 
comp.  (Curie,  Dissert.  1903.) 

Rubidium  carbonate,  Rb2CO3. 

Very  deliquescent,  and  sol.  in  H?O.  100 
pts.  absolute  alcohol  dissolve  0.74  pt.  Rb2CO3. 
(Bunsen.) 

Rubidium  hydrogen  carbonate,  RbHCO3. 

Not  deliquescent.  Easily  sol.  in  H2O. 
(Bunsen.) 


Samarium  carbonate,  Sm2(CO2)3+3H2O. 

Insol.  in  H2O.  (Cleve,  Bull.  Soc.  (2)  43. 
168.) 

Samarium    sodium    carbonate,    Sm2(CO3)3, 

Na2CO3+16H2O. 
Ppt.    (Cleve.) 

Scandium  carbonate,  Sc2(CO3)3  +  12H2O. 
(Crookes,  Roy.  Soc.  Proc.  1908,  80,  A.  518.) 

Scandium  sodium  carbonate,  Sc2(C03)8, 
4Na2CO3+6H2O. 

Difficultly  sol.  in  H2O. 

Sol.  in  cold,  less  sol.  in  hot  alkali  carbonates 
+Aq.  (R.  Meyer,  Z.  anorg.  1910,  67.  410.) 

Silver  carbonate,  Ag2CO3. 

Somewhat  sol.  in  H2O.  Sol.  in  31,978  pts. 
H2O  at  15°.  (Kremers,  Pogg.  85.  248.)  1  g. 
Ag2C03  dissolves  in  2  1.  boiling  H2O.  (Joulin, 

A.  ch.  (4)  30.  260.) 

Solubility  in  H2O  at  25°  =  1.16  x  10-1 
mol.ll.  (Spencer  and  Le  Pla,  Z.  anorg.  1910, 
65.  14.) 

1  1.  H2O  at  25°  dissolves  1.2  x  10-4  gram 
atoms  of  silver.  (Abegg  and  Cox,  Z.  phys. 
Ch.  1903,  46.  11.) 

Insol.  in  H2CO3+Aq.  (Bergman.)  Sol.  in 
961  pts.  H2CO3+Aq.  (Lassaigne.)  1  1.  sat. 
H2CO3+Aq  dissolves  0  846  g.  Ag2CO3  at  15°. 
(Johnson,  C.  N.  54.  75.) 

Sol.  in  (NH4)2CO3+Aq  or  NH4OH+Aq; 
si.  sol.  in  K2CO3+Aq.  (Wittstein.)  Easily 
sol.  in  Na2S2O3+Aq.  (Herschel,  1819.)  Sol. 
in  hot  NH4Cl+Aq,  and  si.  sol.  in  NH4NO3  + 
Aq.  (Brett,  1837.)  Not  pptd.  in  presence  of 
Na  citrate.  (Spiller.)  Decomp.  by  HC1+ 
Aq,  and  chlorides+Aq. 

Somewhat  sol.  in  cone.  NaNO3+Aq.  (de 
Coninck,  Belg.  Acad.  Bull.  1909,  333.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Insol.  in  alcohol. 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 

B.  1910,  43.  314.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Silver  carbonate  ammonia. 

Easily  sol.  in  H2O.  Sol.  in  NH4OH+Aq, 
from  which  it  is  precipitated  by  absolute  al- 
cohol. (Berzelius.) 

Ag2CO3,  4NH3.  Ppt.  Insol.  in  alcohol. 
(Keen,  C.  N.  31.  231.) 

Sodium  carbonate,  Na2CO3. 

Anhydrous.  Sol.  in  H2O  with  evolution  of 
heat. 

Sol  in  5.967  pts.  HzO  at  15°.  (Fresenius.)  100  pts. 
H2O  at  14.6°  dissolve  7.74  pts.  Na^CCs,  or  20.64  pis. 
NasCOs  lOHzO  is  sol.  in  rather  loss  than  1  pt.  boiling 
HzO  (Thomson,  1831.) 

Sol.  in  2  pts.  H2O.     (Bergman. > 

Sol   in  2  pts.  H20  at  18.75°.     (A hi.) 


204 


CARBONATE,  SODIUM 


Solubility  in  100  pts.  H2O  at  t°. 


t° 

Pts. 

Na2C03 

Pts. 
NazCOs 
+  10H2O 

t 

Pts. 
NazCOs 

Pts. 
NajCOs 
+  10H20 

0 
10 
20 

7.08 
16.66 
30  83 

21.52 
61.98 
123.12 

25 
30 
104.6 

35.90 
35.90 
48.50 

171.33 
241.57 

420.68 

(Poggiale,  A.  ch.  (3)  8.  468.) 


Possesses  four  different  degrees  of  solubil- 
ity, according  to  different  states  of  molecular 
constitution  and  degrees  ot  hydration.  (Lowel. 
A.  ch.  (3)  44.  330.) 

Little  more  sol.  at  34-38°  than  at  104°,  but 
maximum  of  solubility  is  probably  at  15°. 
(Lowel.) 


Solubility  of 


,  Na2CO3+10H2O,  Na2CO3+7H2O  (a),  and  Na2C03+7H2O  (6)  in  H2O. 


t° 

Sat.  solution  of 
NazCO.rflOHaO 
contains  — 

Sat.  solution  of 
NazCO3+7H2O  (6) 
contains  —  • 

Sat.  solution  of 
Na2COs+7H20  (a) 
contains  — 

Pts. 
NazCOs  in 
lOOpts.  H20 

Pts. 
Na2CO3  + 
10H2O  in 
lOOpls.  HzO 

Pts. 
NazCOa  in 
100  pts.  H2O 

Pts. 
Na2CO3  + 
7H20  (6)  in 
100  pts.  H2O 

Pts. 
Na2C03  + 
10H2O  in 
100  pts.  H2O 

Pts. 
Na2COa  in 
100  pts.  HzO 

Pis. 
Na2COs  + 
7H2O  (a)  in 
lOOpls.  HzO 

Pts. 
Na2COs  + 
10H2O  in 
100  pts.  H2O 

0 
10 
15 
20 
25 
30 
38 
104 

6.97 
12.06 
16.20 
21.71 
28.50 
37.24 
51.67 
45.47 

21.33 
40.94 
63.20 
92.82 
149.13 
273.64 
1142.17 
539.63 

20.39 
26.33 
29.58 
38.55 
38.07 
43.45 

58.93 
83.94 
100.00 
122.25 
152.36 
196.93 

84.28 
128.57 
160.51 
210.58 
290.91 
447.93 

31.93 
37.85 
41.55 
45.79 

112.94 
150.77 
179.90 
220.20 

188.37 
286.13 
381.29 
556.71 

(Lowel,  A.  ch.  (3)  33.  382.) 


100  pts.   H2O   at   14°  dissolve  60.4  pts. 

Na2CO3  +  10H2O;  at  36°,  833  pts.;  at  104°, 

445  pts.     Solubility  increases  to  36°,  then 

diminishes.    (Payen,  A.  ch.  (3)  43.  233.) 

There  are  apparently  two  maxima  of  solu- 
bility; the  one  occurring  at  15°,  or  even  lower, 

as  warm  solutions  cool;  the  other  at  34-38°, 

when  cold  solutions  are  warmed.     (Payen. 

A.  ch.  (3)  44.  330.) 

Solubility  in  ICO  pts.  H2O  at  t°. 

Pts. 

Pts. 

Pts. 

t 

Na2COs 

t 

NazCOs 

t° 

NazC03 

0 

7.1 

22 

23.8 

43 

46.2 

1 

7.5 

23 

25.1 

44 

46.2 

2 

7.8 

24 

26.5 

45 

46.2 

3 

8.4 

25 

28.0 

46 

46.2 

4 

8.9 

26 

29.7 

47 

46.2 

5 

9.5 

27 

31.6 

48 

46.2 

6 

10.0 

28 

33.6 

49 

46.2 

7 

10.6 

29 

35.8 

50 

46.2 

8 

11.2 

30 

38.1 

51 

46.2 

9 

11.9 

31 

41.4 

52 

46.2 

10 

12.6 

32 

46.2 

53 

46.2 

11 

13.3 

32.5 

59.0 

54 

46.2 

12 

14.0 

33 

46.2 

55 

46.2 

13 

14.8 

34 

46.2 

56 

46.2 

14 

15.6 

35 

46.2 

57 

46.2 

15 

16.5 

36 

46.2 

58 

46.2 

16 

17-.  4 

37 

46.2 

59 

46.2 

17 

18.3 

38 

46.2 

60 

46.2 

18 

19.3 

39 

46.2 

61 

46.2 

19 

20.3 

40 

46.2 

62 

46.2 

20 

21.4 

41 

46.2 

63 

46.2 

21 

22.6 

42 

46.2 

64 

46.2 

Solubility  in  100  pts.  H2O  at  t°— Continued 


t° 

Pts. 
Na2C03 

t° 

Pts. 
NazCOs 

t° 

Pts. 
Na2CO3 

65 

46.2 

79 

46.2 

93 

45.6 

66 

46.2 

80 

46.1 

94 

45.6 

67 

r46.2 

81 

46.1 

95 

45.6 

68 

46.2 

82 

46.1 

96 

45.6 

69 

46.2 

83 

46.0 

97 

45.5 

70 

46.2 

84 

46.0 

98 

45.5 

71 

46.2 

85 

45.9 

99 

45.5 

72 

46.2 

86 

45.9 

100 

45.4 

73 

46.2 

87 

45.8 

101 

45.4 

74 

46.2 

88 

45.8 

102 

45.3 

75 

46.2 

89 

45.8 

103 

45.3 

76 

46  2 

90 

45.7- 

104 

45.2 

77 

46.2 

91 

45.7 

105 

45.1 

78 

46.2 

92 

45.7 

... 

(Mulder,  Scheik.  Verhandel.  1864.  129.) 


Liable  to  form  supersaturated  solutions. 

Supersat.  Na2CO3+Aq  (2  pts.  Na2CO3, 
10H2O:  1  pt.  H20)  may  be  kept  in  a  flask 
closed  with  cotton  wool.  (Schroder.) 

When  supersat.  Na2CO3+Aq  is  exposed  to 
low  temperatures;  the  10H20  salt  crystallizes 
out;  but  under  other  circumstances  two  other 
salts  are  formed,  each  containing  7H2O;  one 
is  four  times  as  sol.  at  10°  as  the  10H2O  salt, 
and  the  other  twice  as  sol.  See  above.  (Lowel, 
A.  ch.  (3)  33.  337.) 

See  also  Na2CO3+H2O,  7H2O,  and  10H2O. 


CARBONATE,  SODIUM 


205 


Sp.  gr.  of  Na2CO3  +Aq  at  15°. 

Sp.  gr.  of  Na2CO3+Aq  at  17.5C. 

%  Na2CO3 

Sp.  gr. 

%  Na2CO3 

Sp.  gr. 

Na2C03 

Na2C03 
+10H2C 

Sp.  gr. 

Na2CO3 

+10H2C 

>  Sp.  gr. 

0.372 
0.744 
1.116 
1.488 
1.850 
2.232 
2.504 
2.976 
3.348 
3.720 
4.090 
4.464 
4.836 
5  .  208 
5.580 
5  .  972 
6.324 
6.396 
6.768 
7  .  440 

1  .  0040 
1.0081 
1.0121 
1.0163 
1  .  0204 
f.0245 
1.0286 
1  .  0327 
1.0368 
1.0410 
1.0452 
1  .  0494 
1.0537 
1  .  0576 
1.0625 
1  .  0669 
1.0713 
1  .  0757 
1.0802 
1  .  0847 

7.812 
8  .  184 
8.556 
8.928 
9.300 
9.672 
10.044 
10.416 
10.788 
11.160 
11.532 
11.904 
12.276 
12.648 
13.020 
13.392 
13.764 
14.136 
14  .  508 
14  .  880 

1.0892 
1.0937 
1.0982 
1  .  1028 
1  .  1074 
1.1120 
1.1167 
1.1214 
1.1261 
1  .  1308 
1  .  1356 
1  .  1404 
1  .  1452 
1.1500 
1-.1549 
1  .  1598 
1  .  1648 
1  .  1698 
1.1748 
1.1816 

1 

2 
3 
4 
5 
6 
7 
8 

2.70 
5.40 
8.10 
10.18 
13.50 
16.20 
18.90 
21.60 

.010 
.020 
.031 
.041 
.052 
.063 
.073 
1.084 

9 
10 
11 
12 
13 
14 
15 

24.30 
27.00 
29.70 
32.40 
35.10 
37.80 
40.50 

1.095 
1.105 
1.116 
1.127 
1.137 
1.148 
1.157 

(Hager.) 

Sp.  gr.   of  Na2CO3+Aq  increases   or  di- 
minishes by  a  change  of  temperature  of  1°  by 
the  following  amounts  — 

(Tiinnerman.) 
Sp.  gr.  of  Na2C03+Aq  at 

15°. 

Corr. 

%  Na2C03 

0.0004 
0.00033 
0.00026 

13-15 

8-12 
3-7 

% 

Sp.  gr.  if  %  is 
Na2C03 

Sp.  gr.  if  %  is 
Na2CO3+10H2O 

(Hager,  Comm.  1883.) 
Sp.  gr.  of  cone.  Na2CO3+Aq  at  30°. 

1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
34 
35 
36 
37 
38 

1.0105 
.0210 
.0315 
.0420 
.0525 
.0631 
.0737 
.0843 
.0950 
.1057 
.1165 
.1274 
.1384 
.1495 

1.004 
1.008 
1.012 
1.016 
1.020 
1.023 
1.027     ' 
.031 
.035 
.039 
.043 
.047 
.050 
.054 
.058 
.062 
.066 
.070 
.074 
.078 
.082 
1.086 
1.090 
1.094 
1.099 
1.103 
1.106 
1.110 
1.114 
1.119 
1.123 
1.126 
1.130 
1.135 
1.139 
1.143 
1.147 
1.150 

Sp.  gr. 

NauCOc 

Na2C03 
in  1  1. 

Sp.  gr. 

1.220 
1.210 
1.200 
.190 
.180 
.170 
.160 
.150 
.140 

Na2COs 

NafcO.3 
in  1  1. 

1.310 
1.300 
1.290 
1.280 
1.270 
1.260 
1.250 
1.240 
1.230 

28.13 
27.30 
26.46 
25.62 
24.78 
23.93 
23.08 
22.21 
21.33 

368.5 
354.9 
341.3 
327.9 
314.7 
301.5 
288.5 
275.4 
262.3 

20.47 
19.61 
18.76 
17.90 
17.04 
16.18 
15.32 
14.47 
13.62 

249.7 
237.3 
225.1 
214.0 
201.1 
18913 
177.7 
166.4 
155.3 

(Lunge,  Chem.  Ind.  1882.  320.) 
Sp.  gr.  of  Na2CO3+Aq  at  23°. 

ii 

Na2COs 

Sp.  gr. 

§3 

NajCOa 

Sp.  gr. 

1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 

0.370 
0.741 
1.112 
1.482 
1.853 
2.223 
2.594 
2.965 
3.335 
3.706 
4.076 
4.447 
4.817 
5.188 
5.558 

1.0038 
1.0076 
1.0114 
1.0153 
1.0192 
1.0231 
1.0271 
1.0309 
1.0348 
1.0388 
1.0428 
1.0468 
1.0508 
1.0548 
1.0588 

16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 

5.929 

6.299 
6.670 
7.04-1 
7.412 
7.782 
8.153 
8.523 
8.894 
9.264 
9.635 
10.005 
10.376 
10.746 
11.118 

.0628 
.0668 
.0708 
.0748 
.0789 
.0836 
.0871 
.0912 
.0953 
1.0994 
1.1035 
1.1076 
1.1117 
1.1158 
1.1200 

CGftrlao.h.  Z. 

anal.  8.  279 

.) 

206 


CARBONATE,  SODIUM 


Sp.  gr.  of  NA2CO3+Aq  at  23°^-Continued. 


31 
32 
33 
34 
35 
36 
37 
38 
39 
40 


Na2C03 


11.488 
11.859 
12.230 
12.60C 
12.971 
13.341 
13.712 
14.082 
14.530 
14.824 


Sp.  gr. 


1.1242 


1.1284 
1 . 1326 
1.1368 
1.1410 
1.1452 
1 . 1494 
1 . 1536 
1.1578 
1.1620 


03O 

S? 


41 
42 
43 
44 

45 

46 
47 
48 
49 
50 


NazCOa 


15.195 
15.556 
15.936 
16.307 
16.677 
17.048 
17.418 
17.789 
18.159 
18.530 


Sp.  gr. 


1.1662 


1704 
1746 


1.1788 


1830 
1873 
1916 
1959 
2002 
2045 


(Schiff,  A.  113.  186.) 

Sp.  gr.  of  Na2CO3+Aq  at  23.3°.  o  =  number 
of  grms.  X  Yz  mol.  wt.,  dissolved  in  1000 
grms.  H20;  6  =  sp.  gr.  if  a  =  Na2CO3, 
10H2O  (Y2  mol.  wt.  =  143);  c=sp.  gr.  if 
o  =  Na2CO3  (%  mol.  wt.=53). 


1.048 
1.086 
1.117 
1.142 


1.052 
1.100 
1.145 
1.187 


1.163 
1.182 
1.198 


1.226 


(Favre  and  Valson,  C.  R.  79.  968). 
Sp.  gr.  of  Na2CO3+Aq  at  18°. 


% 

N7a2CO3 

Sp.gr. 

% 

NazCOs 

Sp.  gr. 

5 
10 

1.0511 
1.1044 

15 

1.1590 

(Kohlrausch,  W.  Ann.  1879.  1.) 
Sp.  gr.  of  Na2CO3+Aq 


g.-equivalents 
Na2C03  per  1. 

t° 

Sp.  gr.  t°/t°. 

0.002524 

16.004 

1.0001418 

0.005041 

16.026 

.0002844 

0.01006 

16.049 

.000568 

0.02501 

16.028 

.001413 

0.04954 

16.050 

.002789 

0.10188 

16.030 

.005699 

0.24646 

16.041 

.013598 

0.002628 

16.051 

.0001473 

0.003948 

16.088 

.0002216 

0.009182 

16.081 

.0005181 

0.01830 

16.089 

1.001033 

0.10842 

16.042 

1.006048 

0.21570 

16.055 

1.011910 

0.4297 

15.14 

1.02346 

2.5015 

16.05 

1.12533 

(Kohlrausch,  W.  Ann.  1894,  53.  26.) 


Sp.  gr.  of  Na2CO3+Aq  at  t°.    H2O  at  4 


60C 


80C 


%  Na2C03 


28.74 
25.20 
22.25 
18.23 
14.06 


28.59 
18.26 


Sp.  gr. 


2971 
2546 
2191 
1746 


1 . 1277 


1.2807 
1.1607 


(Wegscheider,  M.  1905,  26.  690.) 

Sp.  gr.  of  dil  Na2CO3+Aq  at  20.004°. 
Conc.=g.  equiv.  Na2CO3  per  1.  at  20.004° 
and  730  mm. 

Sp.  gr.  compared, with  H2O  at  20.004°  =  !. 


Cone. 

Sp.  gr. 

o.ooco 

1.000,000,0 

0.0001 

1.000,005,6 

0.0002 

1.000,011,2 

0.0004 

1.000,022,5 

0.0005 

1.000,C28,1 

0.0010 

1.000,056,3 

0.0020 

1.000,112,7 

0.0040 

1.000,225,8 

0.0050 

1.000,282,4 

0.0100 

1.000,564,8 

(Lamb  and  Lee,  J.  Am.  Chem.  Soc,  1913,  35. 
1685.) 

Na2CO3+Aq  containing  5%  Na2CO3  boils 
at  100.5°;  10%  Na2CO3,  at  101.1°:  15% 
Na2CO3,  at  101.8°.  (Gerlach.) 

Sat.  solution  boils  at  104.4°  (Griffiths, 
1825);  106°  (Kremers);  104°.  (Payen.) 

Sat.  solution  forms  a  crust  at  104.1°,  and 
contains  42.2  pts.  Na2CO3  to  100  pts.  H2O; 
highest  temperature  observed,  105°.  (Ger- 
lach, Z.  anal.  26.  427.) 

B.-pt.  of  Na2CO3+Aq  containing  pts.  Na2CO3 
to  100  pts.  H2O.  G  =  according  to  Ger- 
lach (Z.  anal.  26.  458);  L  =  according  to 
Legrand  (A.  ch.  (2)  59.  426). 


B.-pt. 


100.5° 

101.0 

101.5 

102.0 

102.5 

103.0 


5.2 
10.4 
15.6 
20.8 
26.0 
31.1 


7.5 

14.4 
20.8 
26.7 
32.0 
36.8 


B.-pt. 


103.5° 

104.0 

104.5 

104.63 

105.0 


36.2 
41.2 
46.2 

51.2 


Less  sol.  in  dil.  NH4OH+Aq  than  in  H2O. 
(Fresenius.) 

See  also  under  Ammonia. 

Solubility  of  Na2CO3+NH4Cl.  See  under 
Ammonium  Chloride. 

Solubility  of  Na2CO3+K2CO3.  See  under 
Carbonate,  potassium. 


CARBONATE,  SODIUM 


207 


The  reciprocal  solubility  of  sodium  car- 
bonate and  sodium  hydrogen  carbonate  in 
H2O  has  been  determined,     (de  Paepe,  C.  A. 
1911,  2603,  and  1912,  2723.) 

Solubility  of  Na2CO3+NaHCO3  in  H2O  at 
25°. 

Solubility  of  Na2CO3+NaBr  in  H2O  at  30°. 

% 

Na2CO3 

% 

NaBr 

Solid  phase 

27.98 
27.54 
26.72 
26.23 
23.40 
22.68 
19.86 
19.57 
18.11 
8.45 
6.90 
3.04 
2.99 
2.60 
0 

0 
2.41 
4.06 
6.26 
11.00 
12.22 
16.88 
16.95 
19.32 
33.39 
36.13 
44.75 
45.31 
45.68 
49.40 

Na2CO3.10H2O 

Na2C03.  1  OH20  +Na2CO3.7H2O 
Na2CO3.7H2O 

Na2C03.7H2O  +Na2CO3.H2O 
Na2CO3.H20 

NaBr.2H2O+Na2CO3.H2O 
NaBr.2H2O 

g.  per  100  g.  H2O 

Solid  phase 

NaHCOs 

Na2CO3 

0 
2.1 
4.2 
5.7 
7.3 
9.0 
10.1 

28.3 
27.3 
26.5 
19.2 
12.4 
6.2 
1.0 

Na2CO3.10H2O 
« 

Na2C03.10H2O+NaHCO3 

NaHCO3 

a 

(i 
K 

(de  Paepe,  Bull.  Soc.  Chim.  Belg.  1911,  25. 

174.) 

Solubility  of  Na2CO3+NaHCO3  in  H2O  at 
25°. 


g.  per  1. 


XaHC03   Na2C03 


98.7 

50.8 
27.6 

0.0 


0.0 
216.6 
276.3 

276.4 


Solid  phase 


>.*        NaHCOa 

NaHC03+Na2CO3,NaHCO3.2H20 
Na2CO3,NaHC03.2H2O  +Na«CO». 

10H2O 
Na2CO3.10H2O 


(McCoy  and  Test,  J.  Am.  Chem.  Soc.  1911 
33.  474.) 

Equilibrium    between    Na2CO3,    NaHCO 


and   CO2. 
hydrogen. 


See   under   Carbonate,    sodium 


Solubility  of  NaNO3  in  Na2CO3+Aq  at  10° 


In  1000  ccm.  H2O 


NaNOa 


805.0 
704.8 


Na2C03 


87.5 
119.8 


Solid  phase 


NaNO3 

NaN03,  Na2CO3 
Na2CO3 


(Kremann,  M.  1909,  30.  325.) 
Solubility  of  NaNO3  in  Na2CO3+Aq  at  24.2' 


In  1000  ccm.  H2O 


NaNO3 


913.58 

844.50 

627.75 

544.3 

459.6 


Na2C03 


59.61 
217.85 
246.30 
263.30 

28.55 


Solid  phase 


NaN03 

K 

NaNO3+Na2CO3.7H2O 


Na2CO3.7H2O 
Na2CO3.10H2O 
Na2CO3.10H2O 


(Kremann.) 


(Cocheret,  Dissert.  1911.) 

Solubility  in  NaCl+Aq.  100  pts.  H2O  dis- 
solve pts.  NaCl  and  pts.  Na2CO  +  10H2O, 
when  that  salt  is  in  excess  at  15°. 


Pts. 
NaCl 


0.00 

4.03 

8.02 

12.02 

16.05 

19.82 


Pts. 

Na2CO3 
+10H20 


61.42 
53.86 
48.00 
43.78 
40.96 
39.46 


Pts. 
NaCl 


23.70 
27.93 
31.65 
35.46 
sat. 
37.27 


Pts. 

Na2C03 
+10H2O 


39.06 
39. 73 
41.44 
43.77 

45.32 


Solubility  of  anhydrous  Na2CO3  in  100  pts. 
NaCl+Aq  containing  %  NaCl  at  15°. 


%  NaCl 


0 
1 

2 
3 

4 

5 

6 

7 

8 

9 

10 

11 


Pts.  Na2C03 


16.408 
15.717 
15.060 
14.438 
13.851 
13.299 
12.783 
12.305 
11.864 
11.461 
11.097 
10.773 


%  NaCl 


12 
13 
14 
15 
16 
17 
18 
19 
20 
21 
22 


Pts.  Na2CO3 

10.488 
10.244 
10.041 
9.880 
9.762 
9.686 
9.655 
9.667 
9.725 
9.828 
9.997 


(Reich,  W.  A.  B.  99,  2b.  433.) 
Solubility  of  Na2CO3-f  NaCl  in  H2O  at  30°. 


Na2CO; 


27.98 
27.48 
27.12 
26.82 
25.59 
24.26 


% 

NaCl 


0 

0.9 
3.33 
4.15 
5.17 
5.93 


Solid  phase 


Na2CO3.10H20 


Na2C03. 10H20  +Na2C03.7H2O 
Na2C03.7H20 


208 


CARBONATE,  SODIUM 


Solubility  of  Na2CO3+NaCl  in  H2O  at 
30°  —  Continued. 

Solubility  of  Na2CO3  in  alcohol  +H2O  at  30°. 

%Na2CO3    %  alcohol 

Solid  phase 

Na2CO 

3     NaCl 

Solid  phase 

27.4           0 
26.61       2.64 
(26.14*     3.411* 
1.38     44.81] 
0.62     52.99 
0.61     53.26 
0.53     55.70 
0.51     56.56 
0.47     62.61 
0.40     63.20 
0.15     72.80 
0.11     73.06 
0.07     78.19 
0.07     82.26 
0.06     86.76 
0.06     90.95 
0.04     93.09 
0.03     95.06 
95.65 
...       98.46 

Na2COs.lOH2O 

Na2CO3.10H2O  +Na2C.O3.7H2O 
Na2C03.7H20 

Na2CO3.7H2O  +Na2CO3.H2O 
Na2COs.H2O 

Na2C03.H20  +Na2C03 
Na2CO3 

22.75 
20.72 
18.00 
14.81 
9.71 
5.05 
0 

10.24 
11.49 
14.12 
16.26 
18.76 
21.94 
26.47 

Na2CO.7H2O  +Na2C03.H2O 
Na2COs.H20 
NaCl+Na2COs.H2O 
NaCl 

(Cocheret,  Dissert.  1911.) 
Solubility  of  Na2C03+NaI  in  H2O  at  30°. 

*  a2CO3 

/al. 

Solid  phase 

27.4 
26.5 
25.5 
25.2 
24.4 
24.3 
23.0 
20.8 
20.0 
18.7 
15.3 
13.1 
10.4 
6.4 
4.2 
3.1 
2.7 
1.5 
0.9 
0.6 
0.3 
0.0 

0 
2.4 
4.7 
5.2 
8.6 
9.5 
11.2 
14.0 
15.7 
18.4 
25.4 
29.1 
33.3 
40.4 
46.0 
49.5 
51.0 
54.6 
57.6 
61.2 
65.6 
65.5 

Na2CO3.10H2O  +Na2CO3.7H2O 
Na2C03.7H20 

Na2.CO3.7H2O-i  Na2CO3.H2O 
Na;CO3.H2O 

NaI.2H20  +Na2C03.H:0 
NaI.2H>0 

*  Conjugated  liquid  phases. 
(Cocheret,  Dissert.  1911.) 
See  also  under  Na2CO8+H2O,  +7H2O  and 
+10H2O. 

Not  decomp.  by  1  pt.  H2SO4+6  pts.  ab- 
solute alcohol. 
Not  decomp.  by  alcoholic  solutions  of  race- 
mi^,  tartaric,  or  glacial  acetic  acids;  slowly 
decomp.  by  HNO3+absolute  alcohol. 
Solubility  of  Na2CO3+NaBr,   NaCl  and 
Nal  in  alcohol.     Numerical  data  given  by 
Cocheret  (Dissert.  1911),  reported  in  Tables 
annuelles  international  es  des  Constants,  etc. 
for  1911. 

Solubility  of  Na2CO3  in  propyl  alcohol  at  20°. 

Alcohol,  wt.  per  cent 

g.  Na2COs  per  100  g. 
solution 

(Cocheret,  Dissert.  1911.) 

Insol.  in  liquid  C02.     (Biichner,  Z.  phys. 
Ch.  1906,  54.  674.) 
Insol.  in  liquid  NH8.    (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 
Insol.  in  alcohol.    (Fresenius.) 
SI.  sol.  in  absolute  alcohol;  apparently  insol. 
in   an  alcoholic  solution  of  soap.     (Duffy, 
Chem.  Soc.  6.  305.) 

Solubility  of  Na2CO3  in  ethyl  alcohol  at  20°. 

28 
38 
44 
46 
48 
50 
54 
62 

4.4 
2.7 
1.7 
1.5 
13 
1.2 
0.9 
0.4 

(Linebarger,  A.  Ch.  J.  1892,  14.  380.) 

A  full  discussion  of  the  solubility  of  Na2C03 
in  propyl,  and  allyl  alcohol  is  given  by  Frank- 
forter  and  Temple  (J.  Am.  Ch.  Soc.  1915,  37. 
2697). 
Insol.  in  CS2.    (Arctowski,  Z.  anorg.  1894, 
6.  257.) 
Insol.  in  benzonitrile.    (Naumann,  B.  1914, 
47.  1370.) 
Insol.  in   methyl   acetate   (Naumann,   B. 
1909,  42.  3790);  ethyl  acetate.     (Naumann, 
B.  1904,  37.  3602.)    ' 

Alcohol,  wt.  per  cent 

g.  Na-COs  per  100  g. 
solution 

44 
46 
48  - 
50 
54 

1.7 
1.13 
0.9 
0.84 
0.80 

(Linebarger,  A.  Ch.  J.  1892,  14.  380.) 

CARBONATE,  SODIUM 


209 


Solubility  in  mixtures  of  pyridine  and  H2O 
from  — 65°  to  +200°.  Solubility  curves  are 
given.  (Limbosch,  Chem.  Soc.  1909,  96  (2), 
472.) 

Insol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

100  g.  glycerine  (sp.  gr.  =  1.262)  dissolve 
98.3  g.  Na2CO3  at  15-16°.  (Ossendowski, 
Pharm.  J.  1907,  79.  575.) 

100  g.  sat.  solution  in  glycol  contain  3.28- 
3.4  g.  Na2CO3.  (de  Coninck,  Bull.  Soc.  Belg. 
1907,  21.  141.) 

100  g.  sat.  Na2CO3+sugar-|-Aq  contain 
6.89  g.  Na2CO3+64.73  g.  sugar  at  31.25°. 
(Kohler,  Z.  Ver.  Zuckerind.  1897,  47.  447.) 

+H2O.  Takes  up  H2O  from  the  air.  Less 
sol.  in  H2O  at  104°  than  at  38°;  at  15-20°,  100 
pts.  H2O  dissolve  52.4  pts.  of  this  salt,  cal- 
culated as  Na2CO3.  Insol.  in  alcohol. 
(Lowel.) 

Solubility  in  100  pts.  H2O  at  t°. 


Corrected  t°. 
(Hydrogen  scale) 

Pts. 
anhydrous  salt 

29.86 

50.53 

29.89 

50.75 

31.80 

50.31 

35.17 

49.63 

35.37 

49.67 

35.66 

49.37 

35.86 

49.44 

36.45 

49.36 

36.90 

49.29 

.37.91 

49.11 

38.92 

49.09 

40.94 

48.51 

40.93 

48.52 

43.94 

47.98 

(Wells  and  McAdam,  J.  Am.  Chem.  Soc.  1907, 
29.  726.) 

Solubility  in  alcohol +Aq. 
Composition  of  the  alcohol  and  water  layers 
in  contact  with  the  solid  phase  Na2CO3+H2O. 


t 

Alcohol  layer 

Water  layer 

% 
alcohol 

% 

salt 

% 

water 

% 
alcohol 

% 

salt 

% 

water 

68 
49 
40 
36 
35 

55.8 
61.0 
61.0 
62.0 
62.9 

0.9 
0.4 
0.4 
0.3 
0.3 

43.3 
38.6 
38.6 
37.7 
36.8 

2.3 
1.2 
1.2 
1.1 
1.0 

28.8 
31.5 
31.9 
32.1 
32.4 

68.9 
67.3 
66.9 
66.8 
66.6 

(Ketner,  Z.  phys.  Ch.  1902,  39.  651.) 

+3H2O.     (Schickendantz,  A.  156.  359.) 
+5H2O.    (Persoz,  Pogg.  32.  303.) 
Not  efflorescent.    Sol.  in  H2O. 
+6H2O.     (Mitscherlich,  Pogg.  8.  441.) 
+7H2O.     Efflorescent.     Two  salts,  7H2O 

(6)  ( =  +  8H2O  of  Thomson),  and  7H2O 

(a).    See  also  under  Na2CO3. 


Solubility  in  100  pts.  H2O  at  t°. 


Corrected  t°. 
(Hydrogen  scale) 


30.35 
31.82 
32.86 
34.37 
34.76 
35.15 
35.17 
35.62 


Pts. 

anhydrous  salt 


43.50 
45.16 
46.28 
48.22 
48.98 
49.23 
49.34 
50.08 


(Wells  and  McAdam,  J.  Am.  Chem.  Soc.  1907, 
29.  726.) 

Composition  of  the  solutions  which  can  be 
in  equilibrium  with  Na2CO3+7H2O/3  at 
different  temperatures. 


32.1 
32.5 
33.3 
33.9 
34.5 


%  Na2C03 


31.8 
32.1 
32.7 
33.0 
33.9 


(Ketner,  Z.  phys.  Ch.  1902,  39.  646.) 

Composition  of  the  alcohol  and  water  layers 
in  contact  with  the  solid  phase,  Na2CO3-f- 
7H2O/8,  at  different  temperatures. 


t° 

Alcohol  layer 

Water  Jayer 

% 
alcohol 

% 

salt 

% 

water 

%al- 
cobol 

% 

salt 

% 

water 

33.2 
32.3 
31.9 
31.45 
31.2 

58.1 
56.1 
54.8 
53.5 
52.4 

0.5 
0.6 
0.7 
0.7 
0.8 

42.4 
43.3 
44.5 
45.8 
46.8 

1.4 
1.5 
1.7 

31.0 
30.2 
29.8 
29.3 
29.3 

67.6 
68.3 
68.5 

(Ketner.) 

Composition  of  the  two  liquid  layers  which 
at  different  temperatures  can  be  in 
metastabile  equilibrium  with  Na2CO3+ 
7H20]8. 


t° 

Alcohol  layer 

Water  layer 

% 
alcohol 

salt 

% 

water 

%  »1- 
cohol 

% 
salt 

•% 
water 

28.9 
.26.6 
23.0 

46.9 

39.1 
24.5 

1.3 
1.3 

6.7 

51.8 
59.6 
68.8 

2.3 
3.3 
7.0 

26.3 
25.4 
20.2 

71.4 
71.3 

72.8 

(Ketner.) 

+10H2O.  Efflorescent.  Sol.  in  1.05  pts. 
H2O  at  23°,  and  sat.  solution  has  sp.  gr. 
1.1995.  (Schiff,  A.  109.  326.) 

Melts  in  crystal  H2O  at  34°.  (Tilden, 
Chem.  Soc.  46.  409.) 

See  above  under  Na2CO3  for  further  data. 


210 


CARBONATE,  SODIUM  HYDROGEN 


Solubility  in  100  pts.  H2O  at  t°. 

Composition  of  the  alcohol  liquids  which  can 
be  in  equilibrium  with  Na2CO3+10H2O 
and   Na2CO3+7H2Oj8  at  different  tem- 
peratures. 

Corrected  t°. 
(Hydrogen  scale) 

Pts. 

anhydrous  salt 

27.84 
29.33 
29.85 
30.35 
31.45 
31.66 
31.72 
32.06 

34.20 
37.40 
38.89 
40.12 
43.25 
43.95 
44.21 
45.64 

t 

%  alcohol 

%  salt 

%  water 

29° 
26° 
21° 

62.3 
67.8 
73.3 

C.3 
0.1 
C.06 

37.4 
32.1 
26.6 

(Ketner.) 

See  also  under  Na2CO3. 
+15H20.    (Jacquelain,  A.  80.  241.) 

/TIT    11       _       J   TV*-  A  J         -       T      A      -     fVL*        .        C(             1  f\f\>-r 

29.  726.) 

Sat.  solution  at  25°  contains  29.37  g.  anhyd. 
Na2CO3  in  100  g.  H2O.  (Osaka,  J.  Tok.  Ch. 
Soc.  1911,  32.  870.) 

Sat.  solution  at  25°  contains  28.3  g.  anhyd. 
Na2CO3  in  100  g.  H2O.  (de  Paepe,  Bull.  Soc. 
Chim.  Belg.  1911,  25.  174.) 

Sat.  solution  at  30°  contains  27.4-27  98  g. 
anhyd.  Na2CO3  in  100  g.  of  the  solution. 
(Cocheret,  Dissert.  1911.) 

Sat.  solution  at  25°  contains  27.64  g.  anhyd. 
Na2CO3  in  100  cc.  of  the  solution.  (McCoy 
and  Test,  J.  Am.  Chem.  Soc.  1911,  33.  474.) 

Solubility  in  alcohol. 

Composition  of  the  alcohol  and  water  layers 
in  contact  with  the  solid  phase,  Na2CO3  + 
10H2O,  at  different  temperatures. 


Alcohol  layer 

Water  layer 

t° 

t» 

°7 

°7 

%  al- 

% 

°7 

alcohol 

salt 

water 

cohol 

salt 

water 

30.6 

47.8 

1.2 

51.0 

2.3 

27.8 

69.9 

29.7 

40.0 

2.1 

57.9 

2.9 

25.5 

71.6 

29.0 

32.7 

3.8 

63.5 

4.3 

22.7 

73.0 

28.2 

23.5 

7.3 

69.2 

7.9 

18.6 

73.5 

(Ketner,  Z.  phys.  Ch.  1902,  39.  651.) 
Solubility  in  alcohol +Aq. 

Liquids  which  can  be  in  equilibrium  with 
Na2C03+10H2Oat21°. 


%  alcohol 

%  salt 

%  water 

0 

18.5 

81.5 

6.2 

12.7 

81.1 

15.3 

6.9 

77  8 

26.1 

3.2 

70  7 

39.2 

1.2 

59  6 

58.2 

0.2 

41.6 

67.1 

0.1 

32.8 

73.3 

0.06 

26.64 

(Ketner.) 


Sodium  hydrogen  carbonate,  NaHCO3. 

100  pts.  cold  H2O  dissolve  7.7  pts.  NaHCOs.  (Rose, 
Schw.  J.  6.  52.) 

100  pts.  H2O  at  11.25°  dissolve  8.27  pts.  NaHCOs  to 
form  solution  of  1.0613  sp.  gr.  (Anthon,  Dingl.  161. 
216.) 

100  pts.  HoO  dissolve  at — 
0°        10°        20°        30° 
8.95     10.04     11.15     12.24  pts.  NaHCO3, 

40°        50°        60°        70° 
13.35     14.45     15.57     16.69  pts.  NaHCO3. 
(Poggiale,  A.  ch.  (3)  8.  468.) 

100  pts.  H2O  dissolve  its.  NaHCO3  at  t°. 


t 

Pts. 
NaHCOs 

t° 

Pts. 
NaHCOs 

t° 

Pts. 
NaHCOs 

0 

6.90 

21 

9.75 

42 

13.05 

1 

7.00 

22 

9.90 

43 

13.20 

2 

7.10 

23 

10.05 

44 

13.40 

3 

7.20 

24 

10.20 

45 

13.55 

4 

7.35 

25 

10.35 

46 

13.75 

5 

7.45 

26 

10.50 

47 

13.90 

6 

7.60 

27 

10.65 

48 

14.10 

7 

7.70 

28 

10.80 

49 

14.30 

8 

7.85 

29 

10.95 

50 

14.45 

9 

8.00 

30 

11.10 

51 

14.65 

10 

8.15 

31 

11.25 

52 

14.85 

11 

8.25 

32 

11.40 

53 

15.00 

12 

8.40 

33 

11.55 

54 

15.20 

13 

8.55 

34 

11.70 

55 

15.40 

14 

8.70 

35 

11.90 

56 

15.60 

15 

8.85 

36 

12.05 

57 

15.80 

16 

9.00 

37 

12.20 

58- 

16.00 

17 

9.15 

38 

12.35 

59 

16.20 

18 

9.30 

39 

12.50 

60 

16.40 

19 

9.40 

40 

12.70 

20 

9.60 

41 

12.90 

(Dibbits,  J.  pr.  (2)  10.  417.) 

Experiments  with  solutions  of  sodium  hy- 
drogen carbonate  show  that  they  gradually 
decompose  after  a  time.  (Treadwell,  Z.  anorg. 
1898,  17.  204.) 

The  source  of  error  of  many  solubility  de- 
terminations of  this  substance  is  due  to  loss 
of  CO2.  Solutions  exposed  to  the  air  lose  CO2. 
(McCoy,  Am.  Ch.  J.  1903,  29.  438.) 

1  1.  sat.  solution  at  25°  contains  98.4  g. 
NaHCO3.  (McCoy  and  Test,  J.  Am.  Chem. 
Soc.  1911,  33.  474.) 


CARBONATE,  SODIUM  HYDROGEN 


211 


NaHCOs+Aq   sat.   at   16°  has  sp.   gr.= 

1/lftQfM        f^tnlhn  ^ 

Temperature,  75°  C. 

.UOyUrt.      [fWOUJn»j 

Nearly  insol.  in  sat.  Nad,  or  Na2SO4+Aq. 
(Balmain,  B.  5.  121.) 

Gram 
atoms  Na 

Amount 
solution  used 
for  titration 

Amount 
Na  combined 
as  NazCOs 

Amount 
Na  combined 
as  NaHCOs 

Equilibrium  between  Na2CO3  and  NaHC03 
in  H2O  and  in  contact  with  the  air. 
System:  Na2CO3,  NaHCO3,  and  CO2. 
Temperature,  25°  C. 

per  liter 

cc. 

Per  cent 

Per  cent 

0.003 

50 
25 
25 

25.7 

74.3 

Amount 

Amount 

Amount  Na 

0.019 

20 

34.8 

65.2 

Gram 

solution  used 

Na  combined 

combined  as 

on 

atoms  Na 
per  liter 

for  titration 
cc. 

as  Na2COs 
Per  cent 

NaHCOs 
Per  cent 

0.036 

£i\J 

10 

55.7 

44.3 

10 

0.0044 

50 

8.7 

91.3 

0.270 

5 

79.5 

20.5 

50 

5 

0.0143 

20 

20.0 

80.0 

0.702 

1 

85.0 

15.0 

20 

1 

0.0562 

10 

37.3 

62.7 

6.56 

1 

84.8 

15.2 

10 

1 

0.2248 

1C 

59.3 

40.7 

0.8847 

10 
2 

64.0 

36.0 

System:  Na2CO3  and  NaHCO3 

at  25°  C. 

2 

0 

Total  salts 

Na2COs                       NaHCOs 

0 

dissolved 

Temperature,  37°  C. 

grams 

Weight 
Grams 

Weight 
Jer  cent      Qra  mg        Per  cent 

Amount 

Amount 

Amount 

0.3555 

0.0203 

5.71      03352    94.29 

Gram 

atoms  Na 
per  liter 

solution  used 
for  titration 

Na  combined 
as  NwCOi 
Per  cent 

Na  combined 
as  NaHCOs 
Per  cent 

1.1053 
4.0443 

0.1505 
1.1041 

13.62      0.9548    86.38 
27.30      2.9402    72.70 

' 

14.6558 

7  0212 

47.91      7.6o 

Ufi    52  09 

0.0019 

50 

10.5 

89.5 

56^3982 

29.8223 

52.88    26.5759    47.12 

O.C071 

50 
20 

20 

21.1 

78.9 

(Cameron  and  Briggs,  J.  phys.  Chem.  1901, 
6.  540.) 

0.0276 

1C 
10 

41.3 

58  7 

100  g.  a  cohol  of  0.941  sp.  gr.  dissolve  1.2  g. 

0   .030 

1C 

64.5 

35.5 

NaHCO3  at  15.5°. 

0.421 

10 
2 

81.9 

18.1 

100  g.  glycerol  dissolve  8  g.  NaHCO3  at 
15.5°.     (Ossendowski,  Pharm.  J.   1907,   79. 

2 

575.) 

0.815 

2 

86.5 

13.5 

Insol.  in  acetone. 

(Naumann,  B.  1904,  37. 

9 

4329.) 

1.795 

2  + 

2 

83.4 

16.6 

Insol.  in   methyl   acetate   (Naumann,   B. 
1909,  42.  3790);  ethyl  acetate.     (Naumann, 

B.  1910,  43.  314.) 

Temperature,  50°  C. 

Insol.  in  acetone  and  in  methylal.     (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

Amount 

Amount 

Amount 

Gram 
atoms  Na 
per  liter 

solution  used 
for  tit  ration 
cc. 

Na  combined 
as  Na2COs 
Per  cent, 

Na  combined 
as  NaHCOs 
Per  cent 

Sodium  rWhydrogen  bicarbonate, 
Na4H2(C00)3+3H20. 

0.0017 

50 

22.2 

77.8 

More  sol.  than  NaHCO3,  less  sol.  tnan 
Na2CO3  in  H2O.    (Rose,  Pogg.  34.  160.) 

0.0071 

25 
20 
20 

32.9 

67.1 

100  pts.  H2O  dissolve,  calculatec 
3C02— 

I  as  2Na20, 

0.0266 

10 

50.7 

49.3 

at    0°     12.63  pts. 

at    60°    29.68  pts. 

20 

10°     15.50 

"    70°     32.55    " 

0.1014 

10 

70.0 

30.0 

20°     18.30 

"    80°     35.8      " 

10 

• 

30°    21.15 

"    90°     38.63     " 

0.4066 

10 

81.0 

19.0 

40°    23.95 

"  100°    41.59     " 

2 

50°    26.78 

0.8068 

2 
2 

86.8 

13.2 

(Poggiale,  A. 

ch.  (3)  8.  468.) 

1.7486 

2.1 

87.1 

12.9 

Min.    Trona,    Urao.      See   Na3H(COa)»-f 

2 

2H20. 

212 


CARBONATE,  SODIUM  HYDROGEN 


Tnsodium  hydrogen  carbonate,  Na3H(CO3)2 
+2H20. 

Sol.  in  H2O. 

True  formula  of  "Trona"  and  "Urao." 
(Zepharovich,  Zeit.  Kryst.  13.  135;  de  Mon- 
desir,  C.  R.  104.  1505.) 

Sodium  thorium  carbonate,  3Na2CO3, 

Th(CO3)2+12H2O. 
Decomp.  by  H2O.    (Cleve.) 

Sodium  uranyl  carbonate,  2Na2CO3, 

(U02)C03. 

Slowly  sol.  in  H2O.  Solution  sat.  at  15°  has 
sp.  gr.  =  1.161.  (Anthon,  Dingl.  166.  207.) 

Sodium  yttrium  carbonate,  Na2CO3,  Y2(CO3)3 

+4H20. 
Ppt.    Not  decomp.  by  cold  H2O.    (Cleve.) 

Sodium  zinc  carbonate,  3Na2O,  8ZnO,  11CO2 

+8H2O  =  3Na2C03,  8ZnCO3+8H2O. 
SI.  decomp.  by  pure  H2O.    (Wohler.) 
Less  easily  decomp.  by  H2O  than  most 

double  carbonates.     (Deville,  A.  ch.  (3)  33. 

101.) 
Na2O,   3ZnO,   4CO2+3H2O.     (Kraut,   Z. 

anorg.  1897,  13.  13.) 

Sodium  carbonate  sulphite,  Na2C03, 2Na2SO3 

+21H20. 

Sol.  in  hot  H2O,  si.  sol.  in  cold  H2O.  (John- 
son, J.  Soc.  Chem.  Ind.  1895,  14.  271.) 

Strontium  carbonate,  SrCO3. 

Sol.  in  18,045  pts.  H2O  at  ordinary  temp. 
(Fresenius.) 

Sol.  hi  12,522  pts.  H20  at  15°.  (Kremers, 
Pogg.  85.  247.) 

Sol.  in  33,000  pts.  H2O.  (Bineau,  C.  R.  41. 
511.) 

Less  sol.  in  H2O  than  SrSO4.    (Dulong.) 

Sol.  in  1536  pts.  boiling  H2O.  (Hope, 
Edinb.  Trans.  4.  5.) 

Calculated  from  electrical  conductivity  of 
SrCO3+Aq,  SrCO3  is  sol.  in  121,760  pts. 
H2O  at  8.8°  and  91,468  pts.  at  24.3°  (Holle- 
mann,  Z.  phys.  Ch.  12.  130). 

1  1.  H2O  dissolves  11  mg.  SrC03  at  18°. 
(Kohlrausch  and  Rose,  Z.  phys.  Ch.  12.  241.) 

"Solubility  product "  =  15. 67  X  10- 10  mol. 
litre.  (McCoy  and  Smith,  J.  Am.  Chem. 
Soc.  1911,  33.  473.) 

Sol.  in  833  pts.  H2CO3+Aq  at  10°. 
(Gmelin.) 

Sol.  in  56,545  pts.  H2O  containing  NH4OH 
and  (NH4)2CO3. 

Quite  sol.  in  NH4Cl+Aq  or  NH4N03-f-Aq, 
but  reprecipitated  on  addition  of  NH4OH  and 
(NH.4)2CO3+Aq.  (Fresenius.) 

Partially  decomp.  by  boiling  with  aqueous 
solutions  of  K2SO4,  Na2SO4,  CaSO4 
(NH4)2S04,  MgS04,  Na2HP04,  (NH4)2HP04 
K2S03,  Na2S03,  (NH4)2S03,  Na2B4O7, 


Na2AsO2,  K2AsO2,  K2C2O4,  Na2C2O4,  NaF, 
and  K2CrO4.  Decomp.  is  complete  with  the 
NH4  salts.  (Dulong,  A.  ch.  82.  286.) 

SI.  decomp.  by  Na2SO4,  or  K2SO4+Aq. 
(Persoz.) 

Easily  sol.  in  NH4  chloride,  nitrate,  or 
succinate+Aq,  but  less  so  than  BaCO3. 
(Fresenius.)  Sol.  in  ferric  salts +Aq,  with 
pptn.  of  Fe2OeH6.  Sol.  in  Na  citrate +Aq. 
(Spiller.)  Not  decomp.  by  a  mixture  of  1  pt. 
H2SO4  and  6  pts.  absolute  alcohol,  or  by  al- 
coholic solutions  of  tartaric,  racemic,  citric, 
or  glacial  acetic  acids;  immediately  decomp. 
by  HNO3+absolute  alcohol,  or  H2C2O4  + 
.  alcohol. 

Solubility  of  SrCO3  in  NH4Cl+Aq. 


abi 


%  NH4C1 

%  SrCOs 

5.35 
10 
20 

0.179 
0.259 
.  0.358 

(Cantoni  and  Goguelia,  Bull.  Soc.  1905,  (3) 
33.  13.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1904,  37.  3602.) 

Insol.  in  acetone.  (Naumann,  B.  1904.  37, 
4329.) 

Insol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

Min.  Strontianite. 

Strontium  hydrogen  carbonate. 

SrC03  is  sol.  in  850  pts.  of  a  sat.  solution  of 
CO2  in  H2O. 

Strontium  uranyl  carbonate,  SrO,  2UO3,  2CO2 

+16H2O. 
As  Ba  comp.    (Blinkoff,  Dissert.  1900.) 

Terbium  carbonate. 

Ppt.  Insol.  in  excess  (NH4)2CO3+Aq. 
(Potratz,  C.  N.  1905,  92.  3.) 

Thallous  carbonate,  T12CO3. 

100  pts.  H2O  dissolve  pts.  T12CO3  (C  =  ac- 
cording to  Crookes;  L  =  according  to  Lamy) 
at— 

15.5°      18°      62°      100°    100.8° 
4.2      5.23     12.85     27.2      22.4  pts.  T12CO3. 
C         L         L          C        L 

Insol.  in  absolute  alcohol  (L),  and  ether  (C). 

Insol.  in  acetone  and  pyridine.  (Naumann, 
B.  1904,  37.  4329.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Thallous  carbonate,  acid,  T12O,  2CO2. 

Rather  easily  sol.  in  cold  H2O.  (Carstan- 
jen.) 


CARBONATE,  ZIRCONIUM 


213 


T1HCO3.  (Giorgis,  Gazz.  ch.  it.  1894,  24. 
474-479.) 

Thallous  carbonate  platinocyanide,  T12CO8, 

Tl2Pt(CN)4. 

SI.  sol.  in  hot,  insol.  in  cold  H2O.  (Fris- 
well,  Chem.  Soc.  (2)  9.  461.) 

Thorium   carbonate,    basic,    2ThO2,    C02-f 

3H20. 

Insol.  in  CO2+Aq,  but  sol.  in  excess  of 
alkali  carbonates  +Aq,  if  cone. 

Tin  (stannous)  carbonate,  2SnO,  CO2. 

Easily  decomp.  on  air;  insol.  in  H2O  or 
H2CO3+Aq.  (Devnie,  A.  ch.  (3)  35.  448.) 

Uranyl   carbonate,    basic,    5(U02)(OH)2, 

3(UO2)CO3+6H2O. 

Ppt.  (Seubert  and  Elten,  Z.  anorg.  1893, 
4.  80.) 

Ytterbium  carbonate,  basic,  Yb(OH)C08+ 

H20. 
Ppt.    (Cleve,  Z.  anorg.  1902,  32.  146.) 

Ytterbium  carbonate,  Yb2(CO8)3+4H2O. 
Ppt.    (Cleve,  Z.  anorg.  1902,  32.  146.) ' 

Yttrium  carbonate,  Y2(CO3)3+3H2O. 

Insol.  in  H2O;  very  si.  sol.  in  H2CO3+Aq. 
Sol.  in  SO2+Aq  and  all  mineral  acids.  Sol. 
in  NH4  salts,  and  alkali  carbonates +Aq  to 
some  extent.  More  sol.  in  (NH4)2CO3-f  Aq 
than  in  K2CO3+Aq.  (Berlin.)  More  sol.  in 
(NH4)2CO3+Aq  than  cerium,  but  5  or  6 
times  less  sol.  than  glucinum  carbonate. 
(Vauquelin.)  Sol.  in  large  excess  of  KHCO3  + 
Aq.  (Rose.)  Slowly  sol.  in  NH4  salts +Aq. 
(Berzelius.) 

Zinc  carbonates,  basic,  8ZnO,  CO2+2H2O; 
5ZnO,  2CO2+3,  or  7H2O;  3ZnO,  CO2  + 
H2O;  HZnO,  4CO2  +  14H2O;  14ZnO, 
5CO2+9H2O;  2ZnO,  CO2+H2O;  8ZnO, 
3CO2+5H2O,  etc. 

All  ppts.  formed  from  Zn  salts  and  carbo- 
nates +Aq.  Sol.  in  2000-3000  pts.  cold  H2O, 
separates  out  on  heating  and  does  not  redis- 
solve  on  cooling.  (Schindler.)  Sol.  in  20,895 
pts.  H2O  at  15°.  (Kremers,  Pogg.  85.  248.) 
Sol.  in  44,600  pts.  H2O  at  ord.  temp.  (Fre- 
senius.) 

Sol.  in  1428  pts.  sat.  H2CO3+Aq.  (Las- 
saigne.)  Sol.  in  189  pts.  H2CO3+Aq  sat.  at 
4-6  atmos.  (Wagner,  Z.  anal.  6.  107.)  Easily 
sol.  in  KOH,  NaOH,  NH4OH,  (NH4)2CO3+ 
Aq,  and  in  acids.  Somewhat  sol.  in  alkali 
bicarbonates  and  NH4  salts +Aq.  (Frese- 
nius.)  Sol.  in  hot  (Fuchs),  also  cold  (Brett, 
1837)  NH4Cl+Aq;  less  sol.  in  NH4NO3+Aq. 
(Brett.) 

Sol.  in  all  NH4  salts +Aq  excepting  (NH4)2S 
+Aq.  (Terreil,  Bull.  Soc.  (2)  9.  441.) 


Insol.  in  Na2CO3,  or  K2CO3+Aq.  Sol.  in 
ferric  salts  -fAq  with  pptn.  of  Fe2O6H6. 
(Fuchs,  1831.) 

The  carbonates  described  by  Boussingault, 
Wackenroder,  Rose,  and  probably  all  salts 
between  ZnO,  CO2  and  5ZnO,  2CO2  are  mix- 
tures. (Kraut,  Z.  anorg.  1897,  13.  1-15.) 

3ZnO,  CO2+2H2O.  Min.  Zinc  bloom,  Hy- 
drozincite. 

ZnCO3,  3ZnO2H2.    Min.  AuricalcUe. 

Zinc  carbonate,  ZnCO3. 

1  1.  H2O  at  15°  dissolves  0.01  g.;  1  1.  H2O 
dissolves  1.64  x  10-4  mols.,  or  0.206  g.  ZnCO3 
at  25°.  (Ageno  and  Valla,  Att.  ace.  Line. 
1911,  20,  II.  706.) 

1  1.  5.85%  NaCl+Aq  dissolves  0.0586  g; 
11. 7.45%  KCl+Aq  dissolves  0.0477  g.  ZnCO,. 
(Essen,  Gm.-K.  4,  1.  680.) 

Sol.  in  acids,  KOH+Aq,  and  NH4  salts -f 

QSol.  inH2CO3-fAq. 

Solubility  hi  various  salts -fAq. 


Solvent 


10%  NaNO3+Aq 
sat.  NaN03+Aq 
5%  NaCl+Aq 

10%  NaCl+Aq 
sat.  NaCl+Aq 

10%  Na2SO4+Aq 
sat.  Na2SO4+Aq 


g.  ZnCOs  sol  in  1  1.  of 
the  solvent 


0.058981 
0.149000 
0.021730 
0.046564 
0.130380 
0.009313 
0.015521 


(Ehlert,  Z.  Elektrochem.  1912,  18.  728.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  830.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

Min.  Calamine,  Smithsonite. 

Calamine  is  sol.  in  NH4OH+Aq  only  in 
the  presence  of  NH4  salts.  (Brandhorst, 
Zeit.  angew.  Ch.  1904,  17.  513.) 

+  ^H2O.    (Mikusch,  Z.  anorg.  1908,  56. 

366.) 

+H2O.    (Belar,  Zeit.  Kryst.  1890, 17.  126.) 

Zinc  carbonate  ammonia,  ZnCO3,  NH3. 

Slowly  decomp.  by  H2O,  but  not  on  the  ah*, 
or  by  boiling  with  alcohol.  (Favre,  A.  ch. 
(3)  10.  474.) 

Zinc   carbonate   hydroxylamine,    ZnCO3, 

2NH3O. 

Insol.  in  H2O.  Decomp.  by  acids.  (Gold- 
schmidt  and  Syngros,  Z.  anorg.  5.  129.) 

Zirconium  carbonate,  3ZrO2,  CO2+6H2O. 

Decomp.  by  hot  H2O,  all  CO2  being  given 
off.  (Hermann.) 

Sol.  in  alkali  carbonates +Aq. 


214 


CARBONIC  ACID 


Percarbonic  acid. 
See  Percarbonic  acid. 

Carbonic  anhydride,  CO2. 
See  Carbon  dioxide. 

Carbonophosphoric  acid. 

Potassium    carbonophosphate,     (K2HP04)2, 

2C02,  2KHC03. 

Known  only  in  solution.  (Barille,  C.  R. 
1903,  137.  566.) 

Carbonyl  bromide,  COBr2. 

Decomp.  by  H,O.  (Besson,  C.  R.  1895, 
120.  192.) 

Carbonyl  platinous  bromide,  CO,  PtBr2. 

Sol.  in  H2O  with  almost  instant  decomp. 
Sol.  in  absolute  alcohol.  (Pullinger,  Chem. 
Soc.  59.  603.) 

Quite  easily  sol.  in  hot  C6H6,  insol.  in 
ligroine,  and  can  be  crystallized  from  CC14. 
Very  easily  sol.  in  HBr+Aq.  (MyHus  and 
Forster,  B.  24.  2432.) 

Carbonyl  bromochloride,  COClBr. 
Decomp.  by  H20.    (Besson.) 

Carbonyl  chloride,  COC12. 

Phosgene.  Cold  H2O  dissolves  1-2  vols. 
COC12  gas  with  slow  decomposition.  Alcohol 
decomp.  immediately.  Immediately  absorbed 
by  KOH,  or  NH4OH+Aq.  Very  sol  in  gla- 
cial HC2H3O2,  benzene,  and  most  liquid  hy- 
drocarbons. (Berthelot,  Bull  Soc.  (2)  13.  14.) 

Sol.  in  SC1«. 

1  vol.  AsCl3  absorbs  10  vols.  COC12. 

ZH'carbonyl  cuprous  chloride,  Cu2Cl2,  2CO  + 

4H20. 

Decomp.  by  air.  (Jones,  Am.  Ch.  J.  1899, 
22.  305.) 

Carbonyl  platinous  chloride,  2COC12,  PtCl2. 
SI.  deliquescent.    Easily  sol.  in  H2O  with- 
out decomp.;  si.  sol.  in  alcohol.    Almost  insol. 
in  CC14.    (Pullinger,  Chem.  Soc.  69.  600.) 

.¥owocarbonyl  platinous  chloride,  CO,  PtCl2. 

Decomp.  by  H2O  and  alcohol;  sol.  in  hot 
CC14.  (Schiitzenberger,  A.  ch.  (4)  15.  100.) 

Sol.  in  cone.  HCl-j-Aq.  (Mylius  and  For- 
ster.) 

Zh'carbonyl  platinous  chloride,  2CO,  PtCl2. 

Decomp.  by  H2O  and  alcohol.  Sol.  in  CC14. 
(Schiitzenberger.) 

Decomp.  by  cone.  HCl+Aq  into  CO  and 
CO,  PtCl2.  (Mylius  and  Forster.) 


Sesquicarbonyl  platinous  chloride,   3CO, 

2PtCl2. 

Decomp.  by  H2O  or  alcohol.  Much  more 
sol.  in  CC14  than  2CO,  PtCl2. 

Carbonyl  platinous  iodide,  CO,  PtI2. 

Not  hygroscopic.  Insol.  in,  but  slowly  de- 
comp. by,  H2O.  Easily  sol.  in  benzene  or 
ether,  also  in  alcohol,  which  decomp.  on  warm- 
ing; sol.  in  HI+Aq.  (Mylius  and  Forster.) 

Carbonyl  platinous  sulphide,  CO,  PtS. 

Easily  decomp.  Insol.  in  ordinary  solvents. 
(Mylius  and  Forster.) 

Carbonyl  sulphide,  COS. 
H20  absorbs  1  vol.  COS. 

Absorption  of  COS  by  H2O  at  t°. 


0 
10 
20 
30 


Coefficient  of  absorption 


1.333 
0.835 
0.561 
0.403 


(Winkler,  Z.  phys.  Ch.  1906,  55.  351.) 

1  ccm.  H2O  at  13.5°  and  756  mm.  pres. 
dissolves  0.8  ccm.  COS.  (Hempel,  Zeit. 
angew.  ch.  1901,  14.  867.) 

1  ccm.  of  a  hydrochloric  acid  solution  of 
Cu2Cl2  absorbs  about  0.2  ccm.  COS.  (Hem- 
pel.) 

Carbonyl  ferrocyanhydric  acid. 

H3Fe(CO)(CN)5. 

Very  sol.  in  H2O;  decomp.  on  heating. 
(Muller,  A.  ch.  (6)  17.  94.) 

Cobalt  carbonyl  ferrocyanide. 

SI.  sol.  in  H2O;  very  sol.  in  dil.  HN03+Aq. 
(M.)  ^ 

Cupric  carbonyl  ferrocyanide, 

Cu3[Fe(CO)(CN)5]2. 
Insol.  in  H2O,  H2SO4,  or  dil.  HNO3-f  Aq. 

(M.) 

Iron  (ferric)  carbonyl  ferrocyanide, 

FeFeCO(CN)5. 

Insol.  in  H20.  Sol.  in  H2C2O4+Aq.  Insol. 
in  acetic,  lactic,  succinic,  tartaric,  and  citric 
acids +Aq,  but  easily  sol.  in  the  neutral  salts 
of  those  acids.  Insol.  in  KC1,  or  KNO3+Aq, 
but  sensibly  sol.  in  Na2HPO4+Aq.  Insol 
even  on  warming  in  very  dil.  H2SO4,  or  H3PO4. 
-fAq.  (Muller.) 

Potassium  carbonyl  ferrccyanide, 

K3Fe(CO)(CN)6+3^H2O. 
100  pts.   H2O   dissolve    148   pts.   at   16°. 
(Muller,  C.  R.  104.  992.) 


CEROUS  HYDROXIDE 


215 


Silver  carbonyl  f errocyanide, 

Ag3Fe(CO)(CN)5. 

Insol.  in  H2O;  si.  sol.  in  dil.  H2S04;  HC1, 
or  HN03+Aq;  scarcely  attacked  by  cone. 
HC2H302+Aq.  (Muller.) 

Sodium  carbonyl  ferrocyanide, 

Na3Fe(CO)(CN)5+6H2O. 
Sol.  inH2O.    (Muller.) 

Uranyl  carbonyl  ferrocyanide, 

(UO2)3[FeCO(CN)6]2+5H2O. 
SI.  sol.  in  H2O,  but  more  easily  if  H2O  is 
acidified  with  HC2H3O2. 

Cericotungstic  acid. 

Ammonium         cericotungstate,     2(NH4)20, 

Ce2O3,  16WO8+2H2O. 
Insol.   in   H2O,   but   decomp.   by   boiling 
therewith.    (Smith,  J.  Am.  Chem.  Sec.  1904. 
26.  1481.) 

Cerium,  Ce. 

Decomp.  pure  H2O  very  slowly  at  ordinary 
temp.  Not  attacked  by  cold  cone.  H2SO4  or 
red  fuming  HNO3.  Sol.  in  dil.  H2SO4+Aq, 
HNO3+Aq,  and  cone,  or  dil.  HCl+Aq. 
(Hillebrand  and  Norton,  Pogg.  155.  633.) 

Cerous  bromide,  CeBr3. 

Anhydrous.  As  the  chloride.  (Robinson, 
Proc.  Roy.  Soc.  37.  150.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4328.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

+zH2O.    Very  deliquescent.    (Jolin.) 

Cerium  gold  bromide,  CeBr3,  AuBr3+8H2O. 
See  Bromaurate,  cerium. 

Cerium  carbide,  CeC2. 

Decomp.  by  fused  alkali  nitrates,  chlorates, 
hydroxides  and  carbonates;  and  by  cone. 
H2SO4  on  heating.  Insol.  in  cone.  HNO3; 
decomp.  by  H2O  and  dil.  acids.  (Moissan, 
C.  R.  1896,  122.  359.) 

CeC3.  Not  attacked  by  hot  cone,  acids. 
(Delafontaine,  J.  B.  1865.  176.) 

Cerous  chloride,  CeCl3. 

Anhydrous.  Deliquescent.  Sol.  in  H2O 
with  hissing  and  evolution  of  heat;  sol.  in 
alcohol. 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4328.) 

Difficultly  scl.  in  methyl  acetate.  (Nau- 
mann, B.  1909,  42.  3790.) 

+7H2O.  Insol.  in  NH4OH-f  Aq.  (Den- 
nis, Z.  anorg.  1894,  7.  260.) 

+73/£H2O.    Deliquescent.    (Berzelius.) 

Decomp.  by  boiling  with  H2O.  Sol.  in  1  pt. 
H2O  at  ord.  temp,  and  3-4  pts.  alcohol. 
(Dumas.) 


Ceric  chloride. 

Known   only   in   solution,    which   decom- 
poses by  slight  heat.    (Berzelius.) 

Cerous  mercuric  chloride. 

Not  deliquescent,    (v.  Bonsdorff.) 
CeCl3,  4HgCl2+10H2O.    Permanent;  eas- 
ily sol.  in  H2O.    (Jolin,  Bull.  Soc.  (2)  21.  533.) 

Cerium  stannic  chloride. 
See  Chlorostannate,  cerium. 

Cerous  chloride  zinc  iodide. 

Sol.  in  H20  and  alcohol.    (Holzmann,  J.  pr_ 
84.  76.) 

Cerous  fluoride,  CeF3. 
Insol.  ppt. 


Ceric  fluoride,  CeF4. 
Insoluble  precipitate.    (Berzelius.) 
+H2O     Insol.  in  H2O.     (Brauner,  B.  14. 

1944.) 

Ceric  cobaltous  'fluoride,  2CeF4,  CoF2+7H2O. 
Ppt.    Easily  decomp.  by  H2O.     (Rimbachv 
A.  1909,  368.  107.) 

Ceric  cupric  fluoride,  2CeF4,  CuF2-f  7H2O. 
Ppt.   Decomp.  by  H2O.    (Rimbach,  L  c.) 

Ceric  nickel  fluoride,  2CeF4,  NiF2-f  7H2O. 
Ppt.    Decomp.  by  H2O.    (Rimbach,  7.  c.) 

Ceric  potassium  fluoride,  2CeF4,  3KF+2H2O. 

Icsol.  in  H2O.  (Brauner,  B.  14.  1944;  15. 
109.) 

Could  not  be  obtained  pure.  (Rimbach, 
/.  c.) 

Ceric  zinc  fluoride,  2CeF4,  ZnF2+7H2O. 
Ppt.    Decomp.  by  H20.    (Rimbach,  L  c.) 

Ceroceric  fluoride,  2CeF8,  CeF4. 
Min.  Fluocerite. 

Cerium  hydride,  CeH2. 

Decomp.  by  acids.    (Winkler,  B.  24.  873.) 
CeH8.    Decomp.  in  moiet  air;  decomp.  by 

hot  or  cold  H2O;  sol.  in  acids  with  evolution 

of  H20.    Decomp.  by  alkalis.    (Muthmann, 

A.  1902,  326.  266.) 

Cerous  hydroxide,  Ce2Os,  zH2O. 

Easily  sol.  in  acids.  Insol.  in  excess  of 
alkali  hydroxides  +Aq.  Sol.  in  (NH4)2CO4+ 
Aq. 

100  ccm.  of  a  solution  in  glycerine  +Aq 
containing  about  60%  by  vol.  of  glycerine 
contain  7.9  g.  Ce2Oa.  (Muller,  Z.  anorg. 
1905,  43.  322.) 

Exists  in  two  modifications:  one  insol.  in 


216 


CERIC  HYDROXIDE 


cold  HCl+Aq;  the  other  sol.  in  cold  HC1+ 
Aq.    (Brauner,  C.  N.  1895,  71.  283.) 

Ceric  hydroxide,  2CeO2,  3H20. 
Sol.  in  HNO8  or  H2SO4;  also  in  HCl+Aq, 

forming  cerous  chloride  and  free  chlorine. 

Insol.  in  hydrofluoric,  acetic,  or  formic  acids + 

Aq.    Somewhat  sol.  in  dil.  HNO8,  or  HC1+ 

Aq.    (Ordway,Am.J.Sci.(2)26.205.)   Insol. 

in  NH4OH,  KOH,  and  NaOH+Aq.    SI.  sol. 

in  alkali  carbonates +Aq.    (Dumas.) 
SI.  sol.  in  (NH4)2CO3+Aq.    (Ordway.) 
100  com.  of  a  solution  in  glycerine +Aq 

containing  about  60%  by  vol.  of  glycerine 

contain  0.08  g.  CeO2.     (Mttller,  Z.  anorg. 

1905,  43.  232.) 

Cerous  iodide,  Gels. 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899,  II. 
1014;  Naumann,  B.  1904,  37.  4328.) 

+9H20.  Very  deliquescent  and  sol.  in 
H2O.  (Lange,  J.  pr.  82.  134.) 

Sol.  in  alcohol. 

Cerium  nitride,  CeN. 

Decomp.  by  H2O  and  alkali.  Sol.  in  min- 
eral acids  with  formation  of  cerous  and  am- 
monium salts.  (Muthmann,  A.  1902,  325. 
272.) 

Cerous  oxide,  Ce2O3. 

When  ignited,  insol.  in  HCl+Aq;  when 
long  digested  with  H2SO4,  is  sol.  in  HCl+Aq 
with  addition  of  alcohol. 

Ceric  oxide,  CeO2. 

When  ignited,  is  only  dissolved  in  traces, 
even  on  heating,  by  HC1  or  HNO3+Aq.  Sol. 
in  cone.  H2SO4  when  warmed.  Sol.  in  the  cold 
in  a  solution  of  Kl  in  HCl+Aq  (Bunsen),  in 
&  mixture  of  HC1  and  FeCl2+Aq,  or  any  re- 
ducing substance. 

Cerium  peroxide,  Ce4O9. 
Insol.  in  boiling  cone,  acids.    Sol.  in  H2SO4 

by  long  digestion.    (Popp,  A.  131.  361.) 
Probably  does  not  exist.     (Rammelsberg, 

Pogg.  108.  40.) 

Ce2O5.    (Hermann,  J.  pr.  30.  184.) 
Probably  does  not  exist.    (Rammelsberg.) 
CeO8+xH2O.     Sol.  in  HCl+Aq.     (Popp, 

A.  131.  361);  (Lecoq  de  Boisbaudran,  C.  R. 

100.  605.) 

Ce02+H2O2,    according   to   Cleve    (Bull. 

Soc.  (2)  43.  57.) 

Cerium  oxycarbide,  CeC2,  2Ce02. 

Stable  in  the  air.  Slowly  attacked  by  cold 
HjO.  With  hot  H20  and  with  acids,  it  gives 
unsat.  hydrocarbons.  (Sterba,  C.  R.  1902, 
134.  1058.) 

Cerium  oxychloride,  CeOCl. 

Slightly  attacked  by  hot  cone.  HCl+Aq. 
Slowly  sol.  in  cone.  HNO3+Aq.  (Wohler.) 


Easily  sol.  in  dil.  acids.    (Didier,  C.  R.  101. 
882.) 

Cerium  oxychloride  tungsten  fn'oxide,  CeOCl, 

WO3. 
(Didier,  C.  R.  102.  823.) 

Cerium  selenide. 

Insol.    in   H2O;   difficultly   sol.   in   acids. 
(Berzelius.) 

Cerium  silicide,  CeSi2. 

Insol.  in  H2O,  by  which  it  is  acted  upon 
only  very  slowly. 


H2. 


in  HC1  and  HF+Aq  with  evolution  of 


Not  attacked  by  alkalis  +Aq  or  NH4OH+ 
Aq. 

Insol.  in  organic  solvents.  (Sterba,  C.  R. 
1902,  136.  170.) 

Cerium  silicide,  Ce2Si8. 

Insol.  in  acids.  (Ullik,  W.  A.  B.  52,  2. 
115.) 

Cerium  bisulphide,  Ce2S4. 

Not  decomp.  by  cold  H2O. 

Slowly  sol.  in  cold  dil.  H2SO4,  HC1  and 
acetic  acid.  Rapidly  sol.  in  warm  dil.  H2S04, 
HC1  and  acetic  acid  with  decomp.  (Biltz,  B. 
1908,  41.  3342.) 

Cerium  sesgmsulphide,  Ce2S3. 

Insol.  in,  and  not  decomp.  by,  H2O,  but 
easily  decomp.  by  the  weakest  acids.  (Mo- 
sander);  (Didier,  C.  R.  100.  1461.) 

Afonochloramine,  NH2C1. 

Easily  sol.  in  H2O.  (Raschig.  Ch.  Z.  1907, 
31.  926.) 

Chlorteframine  comps. 
See  Chlorotetramine  comps. 

Metachlorantimonic  acid,  HSbCl6  + 


Hydroscopic.  Sol.  in  H2O  with  decomp.; 
sol.  in  alcohol,  acetone,  and  acetic  acid. 
(Weinland,  Z.  anorg.  1905,  44.  43.) 

Metachlorantimonic  acid  ammonia,  HSbCle, 

2NH3. 

Sol.  in  H2O  and  in  alcohol.  (Weinland  and 
Schmid,  Z.  anorg.  1905,  44.  59.) 

Aluminum  wefachlorantimonate,  Al(SbCle)» 
+15H20. 

Hydroscopic. 

Sol.  in  dil.  HCl+Aq.  (Weinland,  B.  1903, 
36.  254.) 


CHLORAURATE,  CERIUM 


217 


Ammonium  raetachlorantimonate,  NH4SbCl6 
+H20. 

Hydroscopic. 

Sol.  in  H2O.  Solution  decomp.  slowly  when 
cold,  rapidly  on  warming. 

Sol.  in  dil.  HC1.  (Weinland,  B.  1903,  36. 
251.) 

Cadmium  wetachlorantimonate  ammonia, 

Cd(SbCl6)2,  7NH3. 

Ppt.  (Weinland  and  Schmid,  Z.  anorg. 
1905,  44.  56.) 

Calcium  raetachlorantimonate,  Ca(SbCl6)2+ 
9F20. 

Hydroscopic. 

Sol.  in  dil.  HCl+Aq.  (Weinland,  B.  1903, 
36.  253.) 

Chromium  raetachlorantimonate,  Cr(SbCl6)3 

+13H2O. 
Hydroscopic.' 
Sol.  in  dil.  HCl+Aq.    (Weinland.) 

Chromium  ort/iochlorantimonate,  CrSbCl8+ 

10H2O. 
Hydroscopic. 
Sol.  in  dil.  HCl+Aq.    (Weinland.) 

Cupric  wetachlorantimonate  ammonia, 

Cu(SbCl6)2,  5NH3. 

(Weinland  and  Schmid,  Z.  anorg.  1905,  44. 
55.) 

Glucinum  we/achloraDtimonate,  Gl(SbClfi)2 
+  10H2O. 

Very  hydroscopic. 

Sol.  in  dil.  HC1.  (Weinland,  B.  1903,  36. 
252.) 

Iron  (ferric)  or^ochlorantimonate,  FeSbCls 
+8H2O. 

Hydroscopic. 

Can  easily  be  cryst.  from  dil.  HCl+Aq. 
(Weinland.) 

Lithium  metochlorantimonate,  LiSbCl6+ 

4H20. 

Very  hydroscopic. 
Sol.  in  dil.  HCl+Aa.    (Weinland,  I.  c.) 

Magnesium   pi/rochlorantimonate,   MgSbCly 

+9H20. 
Hydroscopic. 
Sol.  in  dil.  HCl+Aq.    (Weinland.) 

Nickel  metachlorantimonate  ammonia, 

Ni(SbCl6)2,  6NH3. 
Sol.  in  H2O.     (Weinland  and  Schmid,  Z. 
anorg.  1905,  44.  57.) 

Potassium  wetachlorantimonate,  KSbCl6+ 
H2O. 

Hydroscopic. 

Sol.  in  H2O.  Solution  decomp.  slowly  when 
cold,  rapidly  when  warmed. 


Sol.  in  dil.  HCl+Aq.  (Weinland,  B.  1903, 
36.  250.) 

Rubidium  metachlorantimonate,  RbSbCl6. 
Hydroscopic. 
Sol.  in  dil.  HCl+Aq.    (Weinland.) 

Silver  raetachlorantimonate  ammonia. 

AgSbCle,  2NH3. 

Decomp.  by  H20.  (Weinland  and 
Schmid.) 

Zinc  melachlorantimonate  ammonia, 

Zn(SbCl6)2,  4NH3. 
(Weinland  and  Schmid.) 

Chlorarsenious  acid. 
See  Arsenyl  chloride. 

Chlorauric  acid,  HAuCl4  +4H2O. 

Sol.  in  H2O,  alcohol,  and  ether. 

Sol.  in  POC13.  (Walden,  Z.  anorg.  1900,  25. 
212.) 

Difficultly  sol.  in  PC13.    (Walden.) 

Cryst.  with  3H2O  as  stated  by  Weber  and 
Schcttlander  and  not  with  4H2O  as  stated  by 
Thomsen.  (Schmidt,  C.  C.  1906,  II.  855.) 

Chloraurates. 

All  chloraurates  are  easily  sol.  in  H20  and 
in  alcohol,  (v.  Bonsdorff,  1829.) 

Ammonium  chloraurate,  NH4AuCl4+H2O. 
Very  easily  sol.  in  H20. 
+2H2O.    Very  easily  sol.  in  H20. 

Barium  chloraurate,  Ba(Auri4)2+zH2O. 

Deliquescent  in  moist  air.  Sol.  in  H2O  and 
alcohol,  (v.  Bonsdorff,  Pogg.  17.  261.) 

Cadmium  chloraurate. 

Not  deliquescent.  Sol.  in  H2O  and  alcohol. 
(v.  Bonsdorff.) 

Caesium  chloraurate,  CsAuCU. 

100  pts.  aqueous  sat.  solution  contain  at: 
10°    20°    30°    40°    50° 
0.5     0.8     1.7     3.2     5.4  pts.  anhydrous  salt, 

60°    70°    80°    90°     100° 
8.2  12.0  16.3  21.7  27.5  pts.  anhydrous  salt. 
(Rosenbladt,  B.  19.  2538.) 

+  ^H2O.  (Wells  and  Wheeler,  Am.  J. 
(3)  44.  157.) 

Calcium  chloraurate,  Ca(AuCl4)2+6H20. 

Deliquescent.  Sol.  in  H20  and  alcohol,  (v. 
Bonsdorff.) 

Cerium  chloraurate,  CeCl3,  AuCl3+10H2O. 

Extremely  deliquescent.  Easily  sol.  in  H2O 
and  absolute  alcohol.  (Holzmann,  C.  C. 
1863.  206.) 

+13H2O.    (John,  Bull.  Soc.  (2)  21.  534.) 


218 


CHLORAURATE,  COBALT 


Cobalt  chloraurate,  Co(AuCl4)2+8H2O. 
Sol.  in  H2O  and  alcohol.    (Topsoe.) 

Didymium  chloraurate,  DiCl3,  AuCJ3-flOH2O. 

Very  deliquescent.     (Cleve,  Bull.  Soc.  (2) 
43.  361.) 

2DiCl,,  3AuCl3+20H2C.    (Cleve.) 

Gadolinium  chloraurate,  GdCl3,  AuCl3  + 

10H2O. 

Sol.  in  H2C.     (Benedicks,  Z.  anorg.  1900, 
22.  404.) 

Lanthanum  chloraurate,  LaCl3,  AuCl3+5H2O. 
Deliquescent  in  moist  air.     Sol.  in  H2O. 
(Cleve,  B.  8.  128.) 

Lithium  chloraurate,  LiAuCl4. 

100  pts.  aqueous  solution  contain  at: 
10°      20°       30°       40° 
53.1      57.7     62.5     67.3  pts.  anhydrous  salt, 


50C 


60' 


70°       80C 


72.0     76.4     81.0     85.7  pts.  anhydrous  salt. 
(Rosenbladt.) 

+2H2O.  (Antony  and  Lucchesi,  Gazz.  ch. 
it.  1890,  20.  601.) 

+4H20.    Not  stable. 

Sol.  in  H2O  and  alcohol.  (Fasbender,  C.  C. 
1894, 1.  409.) 

Magnesium  chloraurate,  Mg(AuCl4)2+8H20. 

Somewhat  deliquescent.  Sol.  in  H2O  and 
alcohol.  (Topsoe.) 

+12H20. 

Manganese  chloraurate,  Mn(AuCl4)2-f 
8H20. 

Deliquescent.     Sol.  in  H20   and  alcohol. 
(Topsoe.) 
+12H2O. 

Nickel  chloraurate,  Ni(AuCl4)2+8H2O. 

Deliquescent.  Sol.  in  H2O  and  alcohol. 
(Topsoe.) 

Potassium  cbloraurate,  KAuCl4. 

Anhydrous.  Very  stable.  (Lainer,  W.  A. 
B.  99,  2b.  247.) 

ICO  pts.  solution  in  H2O  contain  at: 

10°        20°        30° 
27.7      38.2      48.7  pts.  anhydrous  salt, 

40°        50°        60° 

59.2      70.0      80.2  pts.  anhydrous  salt. 
(Rosenbladt,  B.  19.  2538.) 

Sol.  in  H2O  and  alcohol;  insol.  in  ether. 
(Fasbender,  C.  C.  1894,  I.  409.) 

1  pt.  is  sol.  in  4  pts.  98%  alcohol.  (Fas- 
bender,  C.  C.  1894,  II.  609.) 

+2H2O.    Efflorescent. 


Praseodymium  chloraurate,  PrCl3,  AuCl3  + 

10H2O. 

Very  sol.  in  H2O;  sol.  in  cone.  HC1.    (von 
Schule..  Z.  anorg.  1898,  18.  354  ) 

Rubidium  chloraurate,  RbAuCl4. 

100  pts.  sat.  RbAuCl4+Aq  contain  at: 
10°     20°    30°    40°    50° 
4.6    9.0     13.4  17.7  22.2  pts.  anhydrous  salt, 

60°    70°    80°    90°  100° 
26.6  31.0  35.3  39.7  44.2  pts.  anhydrous  salt. 
(Rosenbladt.) 

1  pt.  sol.  in  54  pts.  98%  alcohol.    Insol.  in 
ether.    (Fasbender,  C.  C.  1894,  II.  609.) 

Samarium  chloraurate,   SmCl3,   AuCl3+ 
10H20. 

Deliquescent.    Easily  sol.  in  H20.    (Cleve, 
Bull.  Soc.  (2)  43.  165.) 

Scandium    chloraurate,     3ScCl3,     2AuCl3+ 
21H2O. 

Very  deliquescent.     (Crookes,  Phil.  Trans. 
1910,  210.  A,  365.) 

Silver  chloraurate,  AgAuCl4. 

Decomp.  in  the  air. 

Decomp.  by  H2O,  HC1  and  NH3.     (Herr- 
mann, B.  1894,  27.  597.) 

Sodium  chloraurate,  NaAuCl4+2H2O. 
Easily  sol.  in  H2O  and  absolute  alcohol. 
100  pts.  aqueous  solution  contain  at: 
10°        20°        30° 
58.2       60.2      64.0  pts.  anhydrous  salt, 

40°        50°        60° 

69.4      77.5      90.0  pts.  anhydrous  salt. 
(Rosenbladt.) 

Easily  sol.  in  NaCl+Aq. 
Easily  sol.  in  H2O,  alcohol  and  ether.  (Fas- 
bender,  C.  C.  1894,  I.  409.) 

Strontium  chloraurate. 
Sol.  in  H2O.    (v.  Bonsdorff.) 

Thallium  chloraurate. 

(Carstanjen.) 

Ytterbium  chloraurate,  YbCl3,  AuCl3+9H2O. 
Ppt.    (Cleve,  Z.  anorg.  1902,  32.  138.) 

Yttrium  chloraurate,  YtCl3,  2AuCl3  +  16H2O. 
Very  sol.  in  H2O.    (Cleve.) 

Zinc  chloraurate,  Zn(AuCl4)2+8H2O. 

Sol.  in  H2O.    (Topsoe.) 

+12H2O.     Sol.  in  H2O  and  alcohol,     (v. 
Bonsdorff.) 


CHLORHYDRIC  ACID 


219 


Chlorauricyanhydric  acid. 

Barium  chlorauricyanide,  Ba[Au(CN)2Cl2]2  + 
8H2O. 

Very  sol.  in  H2O  or  alcohol.  (Lindbom, 
Lund  Univ.  Arsk.  12.  No.  6.) 

Potassium  chlorauricyanide,  KAu(CN)2Cl2  + 

H2O. 
Very  sol.  in  H2O  or  alcohol. 

Strontium  chlorauricyanide,  Sr[Au(CN)2Cl2]2 

-f-8H2O. 
Sol.  in  H2O. 

Zinc     chlorauricyanide,    Zn[Au(CN)2Cl2]2  + 

7H2O. 
Very  sol.  in  H20. 

Chlorhydric  acid,  HC1. 

Liquid.    Miscible  with  liquid  CO2,  and  H2S. 

Gas.  Absorbed  by  H2O  with  production  of 
much  heat. 

H2O  absorbs  400-500  vols.  at  ord.  temp,  and  pressure 
or  a  little  less  than  1  pt.  by  weight.  (Dalton.) 

1  vol.  H2O  absorbs  480  vols.  at  0°;  sp.  gr.  of  sat  solu- 
tion is  1.2109.  (Davy.) 

1  vol.  H2O  absorbs  417  822  vols.  at  20°,  the  vol.  in- 
creasing to  1.4138  vols.;  1  vol.  of  HCl+Aq  then  con- 
tains 311  vols.  HC1,  has  sp.  gr.  1.1958.  and  contains 
40.39%  HC1  by  weight.  (Thomson,  1831.) 

1  vol.  H2O  absorbs  464  vols.  and  sat.  solution  has  1.21 
sp.  gr.  and  contains  42.4%  HC1  by  weight.  (Wittstein.) 

H2O  sat.  at  0°  contains  480  times  its  vol.  of  HC1.  and 
sp.  gr.  =1.2109:  sat.  at  ord.  temp.,  contains  38.3%  of 
its  weight  in  HC1,  and  sp.  gr.  =1.192.  (Berzelius.) 

1  vol.  H2O  absorbs  V  vols.  HC1  at  t°  and  760  mm. 
pressure,  and  the  liquid  foimed  has  the  given  sp.  gr., 
and  contains  the  given  per  cent  HC1. 


t° 

V 

Sp.  gr. 

%HC1 

o 

4 
8 
12 
14 
18 
18.25 
23 

525.2 
494.7 
480.3 
471.3 
462.4 
451.2 
450.7 
435.0 

1  .  2257 
.2265 
.2185 
.2148 
.2074 
.2064 
1  .  2056 
1  .  2014 

45.148 
44.361 
43.828 
43.277 
42.829 
42  .  344 
42  .  283 
41.536 

(Deicke,  Pogg.  119.  156,) 

At  760  mm.  pressure  1  g.  H2O  absorbs 
g.  HCl  at  t°. 


t 

g.  HCl 

t° 

g   HCl 

t° 

g.  HCl 

0 

0.825 

22 

0.710 

44 

0.618 

2 

0.814 

24 

0.700 

46 

0.611 

4 

0.804 

26 

0.691 

48 

0.603 

6 

0.793 

28 

0.682 

50 

0.596 

8 

0.783 

30 

0.673 

52 

0.589 

10 

0.772 

32 

0.665 

54 

0.582 

12 

0.762 

34 

0.657 

56 

0  575 

14 

0.752 

36 

0.649 

58 

0.568 

16 

0.742 

38 

0.641 

60 

0.561 

18 

0.731 

40 

0.633 

20 

0.721 

42 

0.626 

(Roscoe  and  Dittmar.) 


Cone.  HCl+Aq  loses  HCl,  and  dil.  HC1+ 
Aq  loses  H2O  on  warming,  until  an  acid  of 
constant  composition  is  formed,  containing 
20.18%  HCl,  with  a  sp.  gr.  of  1.101  at  15°, 
which  can  be  distilled  unchanged  at  110°. 
(Bineau,  A.  ch.  (3)  7.  257.) 

The  above  is  true  if  barometer  is  at  760 
mm.,  but  the  composition  changes  with  the 
pressure  as  follows — 


Mm. 
Hg 

%  HCl 

Mm. 
Hg. 

%HC1 

Mm. 
Hg 

%HC1 

50 

23.2 

800 

20.2 

1700 

18.8 

100 

22.9 

900 

19.9 

1800 

18.7 

200 

22.3 

1000 

19.7 

1900 

18.6 

300 

21.8 

1100 

19.5 

2000 

18.5 

400 

21.4 

1200 

19.4 

2100 

18.4 

500 

21.1 

1300 

19.3 

2200 

18.3 

600 

20.7 

1400 

19.1 

2300 

18.2 

700 

20.4 

1500 

19.0 

2400 

18.1 

760 

20.24 

1600 

18.9 

2500 

18.0 

(Roscoe  and  Dittmar.) 

Cone.  HCl+Aq  gradually  gives  off  HCl  on 
the  air  until  it  has  a  sp.  gr.  1.128  at  15°,  and 
contains  25.2%  HCl.  (Bineau,  I.  c.) 

According  to  Roscoe  and  Dittmar,  this  de- 
pends on  the  temperature.  If  a  current  of  ah* 
is  passed  through  HCl+Aq,  acid  or  water 
is  given  off  according  as  the  acid  is  strong  or 
weak,  until  an  acid  of  constant  composition 
for  a  given  temperature  is  formed,  as  follows — • 


Temp. 

%  HCl 

Temp. 

%  HCl 

Temp. 

%  HCl 

0° 

25.0 

35° 

23. 

9 

70° 

22.6 

5 

24.9 

40 

23. 

8 

75 

22.3 

10 

24.7 

45 

23.6 

80 

22.0 

15 

24.6 

50 

23.4 

85 

21.7 

20 

24.4 

55 

23. 

2 

90 

21.4 

25 

24.3 

60 

23. 

0 

95 

21.1 

30 

24.1 

65 

22. 

8 

100 

20.7 

From  the  above  it 

is  seen 

that  the  acid 

which  distils  unchanged  at  a  given  pressure, 
that  is,  boils  at  a  certain  constant  tempera- 
ture, is  identical  with  the  acid  which  under- 

goes no  change  in  composition  by  a  current 
of  dry  air  at  the  same  temperature,  and  under 
the  ordinary  pressure,  thus  — 

Mm. 
Hg 

B.-pt. 

%  HCl 

Temp,  of 
air  current 

%HCI 

100 

61-62° 

22.8 

62° 

22.9 

200 

76-77 

22.1 

77 

22.2 

300 

84-85 

21.7 

85 

21.7 

380 

91 

21.3 

91 

21.4 

490 

97 

20.9 

< 

)8 

21.1 

620 

103 

20.6 

fRosnop  n.nrl  Ditfmnr  ^ 

220 


CHLORHYDRIC  ACID 


Solubility  of  HCl  in  H2O  at  0°  under  different 
degrees  of  pressure.    P  =  partial  pressure 
in  mm.  Hg,  i.  e.,  total  pressure  minus  the 
tension  of  aqueous  vapour  at  the  given 
temp.;  G  =  grammes  of  HCl  dissolved  in 
1  g.  H2O  at  the  pressure  P  and  0°  temp. 

Sp.  gr.  of  HCl-fAq. 

Sp.  gr. 

%HC1 

Sp.  gr. 

%HC1 

Sp 

•  gr. 

%HC1 

1.203 
1.179 
1.162 
1.149 
1.139 

40  .  66 
37.00 
33.95 
31.35 
29.13 

1  .  1285 
1.1197 
1.1127 
1  .  1060 
1  .  1008 

27.21 
25  .  52 
24.03 
22.70 
21.51. 

1  .  0960 
1  .  0902 
1.0860 
1  .  0820 
1  .  0780 

20.44 
19.47 
18.59 
17.79 
17.05 

P 

G 

P 

G 

(Thomson,  in  his  System,  2.  189.) 
Sp.  gr.  of  HCl  +Aq. 

60 
70 
80 
90 
100 
110 
120 
130 
140 
150 
175 
200 
225 
250 
275 
300 

a.  613 

0.628 
0.640 
0.649 
0.657 
0.664 
0.670 
0.676 
0.681 
0.686 
0.697 
0.707 
0.716 
0.724 
0.732 
0.738 

350 
400 
450 
500 
550 
600 
650 
700 
750 
800 
900 
1000 
1100 
1200 
1300 

0.751 
0.763 
0.772 
0.782 
0.791 
0.800 
0.808 
0.817 
0.824 
0.831 
0.844 
a.  856 
0.869 
0.882 
0.895 

Sp.  gr. 

%HC1 

Sp.  gr. 

%HC1 

1.21 
1.20 
1.19 
.18 
.17 
.16 
.15 
.14 
.13 
.12 
.11 

42.43 
40.80 
38  .  38 
36.36 
34.34 
32.32 
30  .  30 
28.28 
26.26 
24.24 
20.30 

1.10 
1.09 
1.08 
1.07 
1.06 
1.05 
1.04 
1.03 
1.02 
1.01 

20.20 
18.18 
16.16 
14  .  14 
12.12 
10.10 
8.08 
6.06 
4.04 
2.02 

(Edm.  Davy.) 
Sp.  gr.  of  HCl  +Aq. 

Sp.  gr. 

%  HCl 

B.-pt. 

Sp.  gr. 

%  HCl 

B.-pt. 

(Roscoe  and  Dittmar,  A.  112.  334.) 

1  vol.  H2O  dissolves  560  vols.  HCl  at  —12° 
"              "        500    "        "              0° 
"              "        440    "        "         +20° 
(Berthelot,  C.  R.  76.  779.) 

1  vol.  H2O  absorbs  480  vols.  HCl  at  15°  to 
form  a  solution  containing  42.85%  HCl  with 
a  sp.  gr.  of  1.215.    (Hager.) 

Solubility  of  HCl  at  low  temperatures,  and 
760  mm.  pressure. 

1.199 
1.181 
1.166 
1  .  154 
1.144 
1.136 
1.127 
1.121 

34.01 
31.09 

28.29 
26.57 
24.84 
23.25 
21.06 
20.74 

49° 
65 
76 
87 
100 
103 
105 
109 

.094 
.075 
.064 
.047 
.035 
.018 
1.009 

16 
13 

11 
8 
6 
3 
1 

.08 
.16 
.16 
.62 
.92 
.52 
.86 

111° 
109 
]07 
105 
104 
102 
101 

(Kirwan  and  Dalton.) 
Sp.gr.  of  HCl  +Aq  at  15°. 

%  HCl 

Sp.  gr. 

%  HCl 

Sp.  gr. 

"t 

Pts.  HCl 
in  1  pt.  H2O 

t° 

Pts.  HCl 
in  1  pt.  H2O 

2.22 
3.80 
6.26 
11.02 
15.20 
18.67 
20.9] 
23.72 
25.96 

.0103 
.0189 
.0310 
.0557 
.0751 
1  .  0942 
1.1048 
1.1196 
1  .  1308 

?9  .  72 
31.50 
34.24 
36.63 
38.67 
40.51 
41.72 
43.09 

1.1504 
1  .  1588 
1  .  1730 
1  .  1844 
1  .  1938 
1.2021 
1  .  2074 
1.2124 

0 
-  5 
-10 
-15 
-17 

0.842 

0.864 
0.898 
0.933 
0.949 

-18 
-19 
-20 
-21 

-24 

0.957 
0.965 
0.974 
0.983 
1.012 

(Roozeboom,  R.  t.  c.  1884,  3.  79.) 
Solubility  in  H2O  at  t°. 

(Kolb,  C.  R.  74.  337.) 

Sp.  gr.  of  HCl  +Aq  at  15°. 

t° 

%HC1 

Sp.  gr. 

%  HCl 

Sp.  gr. 

%  HCl 

Sp.  gr. 

%HC1 

50 
45 
40 
35 
30 
20 
15 
10 
5 
0 
-  5 
-10 
-50 
-20 

61.65 
61.76 
62.27 
62.90 
63.21 
64.19 
64.70 
65.18 
65.48 
65.85 
66.44 
66.71 
67.29 
67.65 

1  .  2000 
1  .  1982 
1  .  1964 
1  .  1946 
1  .  1928 
1.1910 
1  .  1893 
1.1875 
1  .  1859 
1  .  1846 
1  .  1822 
1  .  1802 
1  .  1782 
1  .  1762 
1.1741 
1.1721 
1  .  1701 
1.1681 
1.1661 
1J641 

40 
40 
39 
39 
39 
38 
38 
37 
37 
37 
36 
36 
35 
35 

34 
34 
33 
33 
33 

777 
369 
961 
554 
146 
738 
330 
923 
516 
108 
700 
292 
884 
476 
068 
660 
252 
845 
437 
029 

.1620 
.  1599 
.  1578 
.1557 
.  1536 
.  1515 
.1494 
.1473 
.  1452 
.1431 
.1410 
.  1389 
.1369 
.1349 
.1328 
.  1308 
.1287 
.1267 
.1247 
.1226 

32.621 
32.213 
31  .  805 
31.398 
30  .  990 
30  .  582 
30.174 
29  .  767 
29.359 
28.951 
28.544 
28.136 
27.728 
27.321 
26.913 
26.505 
26  .  098 
25  .  690 
25  .  282 
24.874 

1  .  1206 
1.1185 
1.1164 
1.1143 
1.1123 
1.1102 
1  .  1082 
1.1061 
1.1041 
1.1020 
1  .  1000 
1  .  0980 
1  .  0960 
1.0939 
1.0919 
1.0899 
1.0879 
1  .  0859 
1.0838 
1.0818 

24  .  466 
24  .  058 
23  .  650 
23  .  242 
22  .  834 
22.426 
22.019 
21  611 
21.203 
20.796 
20.288 
19.980 
19  .  572 
19.165 
18.757 
18.349 
17.941 
17.534 
17.126 
16.718 

(Rupert,  J.  Am.  Chem.  Soc.  1909,  31.  860.) 

CHLORHYDRIC  ACID 


221 


Sp.  gr.  of  HCl+Aq  at  15°  —  Continued. 

Sp.  gr.  of  HCl+Aq  at  15°. 

Sp.  gr.     %  HCl 

Sp.  gr. 

%HC1 

Sp.  er 

%HC1 

HCl 

Sp.  gr. 

HCl 

Sp.  gr. 

ric.      Sp"  gr' 

1.0798     16.310 
1.0778     15.902 
1.0758     15.494 
1.0738     15.087 
1.0718     14.679 
1.0697     14.271 
1.0677     13.363 
1.0657     13.456 
1.0637     13.409 
1.0617     12.641 
1  .  0597     12  .  233 
1.0577     11.825 
1.0557     11.418 
1.0537     11.010 

1.0517 
1  .  0497 
.0477 
.0457 
.0437 
.0417 
.0397 
.0377 
.0357 
.0337 
.0318 
1.0298 
1  .  0279 

10.602 
10.194 
9.768 
9.379 
8.971 
8  .  563 
8  .  1  £5 
7.747 
7.340 
6.932 
6.524 
6.116 
5.709 

1  .  0259 
1  .  0239 
1  .  0220 
1  .  0200 
1.0180 
1.0160 
1.0140 
1.0120 
1.0100 
1  .  0080 
1  .  0060 
1  .  0040 
1.0020 

5.301 
4.893 
4.486 
4  .  078 
3.670 
3.262 
2.854 
2.447 
2.039 
1.631 
1.224 
0  .  816 
0.408 

5 
10 
15 

1.0244 
1  .  0488 
1.0733 

20 
25 
30 

1  0982 
1.1234 

1  .  1488 

35       1  1739 
40       1.1969 
41       1.2013 

(Hager,  Adjumenta  varia,  Leipzig,  1876.) 
Sp.  gr.  of  HCl+Aq  at  15°  (H2O  at  15°=  1). 

%  HCl             Sp.  gr. 

%HC1              Sp.  gr. 

(Ure,  Hand? 

Sp.  gr.  of  HCl+Aq. 
according  to  Ure; 
cording  to  Kremei 

/6i  terbuc 

h.) 

.  gr.  at  15.55° 
gr.  at  15°  ac- 

U-sp 
K=sp 

s. 

44. 
43. 
41. 
41. 
39. 
37. 

345       1.21479 
136       1.21076 
901        1.20430 
212       1.20204 
831        1.19703 
596        1.18687 

34.464       1.17138 
25.260       1.12479 
19.688       1.09675 
14.788       1.07255 
6.382       1.03150 

%HC1 

u 

K 

%HC1 

u 

K 

1 

2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
21 

1.005 
010 
015 
.020 
.025 
.030 
.034 
.039 
.044 
.048 
.053 
.059 
.064 
.069 
.074 
.079 
1.084 
1.089 
1.094 
1  098 
1.104 

.005 
010 
.015 
020 
.025 
.030 
1.034 
1.039 
1.044 
1.048 
1.053 
1.059 
1  065 
1.070 
1.075 
1.080 
1.085 
1  090 
1.095 
1.100 
1.105 

22 
23 
24 
25 

26 
27 
28 
29 
30 
31 
32 
33 
34 
35 
36 
37 
38 
39 
40 
41 

1  109 
1  114 
1  119 
1  124 
1  128 
1  133 
1  138 
1  143 
1  147 
1  153 
1  157 
1  163 
1  169 
1  174 
1  179 
1  183 
1  188 
1  193 
1  197 
1  203 

1.111 

1.116 
1.121 
1.126 
1.131 
1.136 
1.141 
1.146 
1.151 
1.157 
1.163 
1.169 
1.179 

(Pickering,  B.  26.  277.) 
Most  accurate  table. 
Sp.  gr.  of  HCl+Aq  at  15°  (H2O  at  4°=  1). 

Sp.  gr. 

%  HCl 

Kg.  HCl 
in  1     . 

Sp.  gr. 

%  HCl 

Kg.HCl 
in  11. 

1.000 
1.0C5 
1.010 
1.015 
1.020 
1.025 
1.030 
1.035 
1.040 
1.045 
1.050 
1.055 
1.060 
1.065 
1.070 
1.075 
1.080 
1.085 
1.090 
1.095 
1.100 

0.16 
1.15 
2.14 
3.12 
4.13 
5.15 
6.15 
7.15 
8.16 
9.16 
10.17 
11.18 
12.19 
13.19 
14.17 
15.16 
16.15 
17.13 
18.11 
19.06 
20.01 

0.016 
0.012 
0.022 
0.032 
0.042 
0.053 
0.064 
0.074 
0.085 
0.096 
0.107 
0.118 
0.129 
0.141 
0.152 
0.163 
0.174 
0.186 
0.197 
0.209 
0.220 

1.105 
1.110 
1.115 
1.120 
1.125 
1.130 
1.135 
1.140 
1.145 
1.15C 
1.155 
1.160 
1.165 
1.170 
1.175 
1.180 
1.185 
1.190 
1.195 
1.2CO 

20.97 
21.92 
22  .  86 
23.82 
24.78 
25.75 
26.70 
27.66 
28.61 
29.57 
30.55 
31.52 
32.49 
33.46 
34.42 
35.39 
36.31 
37.23 
38.16 
39.11 

0.232 
0.243 
0.255 
0.267 
0.278 
0.291 
0.303 
0.315 
0.322 
0.340 
0.353 
0.366 
0.379 
0.392 
0.404 
0.418 
0.430 
0.443 
0.456 
0.469 

(Calculated  by  Gerlach,  Z.  anal.  8.  292.) 
Sp.  gr.  of  HCl+Aq  at  15°  (H2O  at  0°  =  1). 

HCl 

Sp.  gr. 

£,    *•; 

Sh 

Sp.  gr. 

0 

1 

2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 

0.9992 
1.00503 
1.01005 
1.01508 
1.02010 
1.02513 
.03016 
.03518 
.04021 
.04524 
.05026 
.  05529 
.06031 
1.06534 
1.07037 

15      1.07539 
16      1.08042 
17      1.08545 
18      1.09047 
19      1.09550 
20      1.10052 
21      1  .  10555 
22      1.11058 
23      1.11560 
24      1.12063 
25      1.12566 
26      1  .  13068 
27      1.13571 
28      1  .  14074 
29      1  .  14516 

30 
31 
32 
33 
34 
35 
36 
37 
38 
39 
40 
41 
42 
43 

1  .  15079 
1  .  15581 
1  .  16084 
1  .  16587 
1  .  17089 
1  .  17592 
1  .  18095 
1  .  18597 
1.191 
1.196 
1.200 
1.204 
1.208 
1.212 

(Lunge  and  Marchlewski,  Z.  angew.  Ch.  1891. 
133.) 

Sp.  gr.  of  HCl+Aq  at  room  temp. 

%HC1 

Sp.  gr. 

8.14 
16.125 
23.045 

1.0370 
1.0843 
1.1138 

(Kolb,  recalculated  by  Gerlach,  Z.  anal.  27. 
316.) 

(Wagner,  W.  Ann.  1883,  18.  264.) 

222 


CHLORHYDRIC  ACID 


Relation  of  sp.  gr.  of  HCl+Aq  at  t°  to  sp.  gr.  at  19.5°  =  1.0. 


t° 

8.9  %  HC1 
sp.gr.  =1.0401 

16  6  %  HC1 
sp.  gr.  =1.0704 

25.5%   HC1 
sp.  gr.  =1.101 

35.8%   HCI 
sp.  gr.  =1.133 

46.6  %  HCI 
sp.  gr.  =1.1608 

0 
19.5 
40 
60 
80 
IOC 

0.99557 
1.00000 
1.00707 
1.01588 
1.02639 
1.03855 

0.99379 
.00000 
.00781 
.01665 
.02676 
.03801 

0.99221 
l.OOOCO 
1.C0877 
1.01794 
1.02791 
1.03867 

0.99079 
1.00000 
1.00990 
'1.01969 
1.C2986 
1.04059 

0.98982 
1.00000 
1.01063 
1.02180 

(Kremers,  Fogg.  108.  115.) 


Sp.  gr.  of  HCl+Aq. 

Sp.gr.  of  HCl  +  Aq 

at  20°. 

G.  equivalents 
HCI  per  liter. 

t° 

Sp.  gr.  t°/t° 

Normality  of 
HCl+Aq. 

%  HCI. 

Sp.  gr. 

0.005036 
0.01006 
6.  02008 
0.04990 
0.09885 
0.19641 
0.29247 
0.48278 
0.4994 
4.994 

17.111 
17.125 
17.148 
17.138 
17.133 
17.162 
17.147 
17.140 
17.28 
17.35 

.  0000943 
.0001892 
.0003775 
.000935 
.001843 
.003633 
.005382 
.008811 
1.00908 
1.08390 

8.42 
5.784 
3.77 
2.031 
1.588 
1.138 
0.523 

27.10 
19.30 
12.94 
7.17 
5.65 
4.05 
1.90 

.1336 
.0936 
.0618 
.0334 
.0261 
1.0187 
1.0076 

(Forchheimer,  Z.  phys.  Ch.  1900,  34.  28.) 

Sp.  gr.  at  20°  of  HCl+Aq  containing  M  g. 
mols.  HCI  per  liter. 
M             0.025        0.05          0.075        0.10 
Sp.gr.    1.00034     1.00101     1.00135     1.00180 

(Kohlrausch,  W.  Ann.  1894,  53.  28.) 
Sp.  gr.  of  a  normal  solution  of  HCl+Aq 

at   18°/4°=  1.0165.      CLoomis    W     Ann     ISQft 

v*V**«         \-**ns\jmta*      TT   .     -tiiAiJ.,     J.O»7v/j 

Sp.  gr.  of  HCl+Aq  at  19.5°,  when  p  =per 
cent  strength  of  solution;  d=  observed 
density;  w  =  volume  cone,  in  grams 


M 

Sp.  gr. 


0.25 
1  .00425 


0.50 
1.00849 


0.75 
1.01264 


1.0 

1.01749 


Per  cc-     ^  = 


M  1.5  2.0 

Sp.gr.    1.02542     1.03414 

(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38.  730.) 


p- 

d. 

W 

36.0 

.1818 

0.4255 

29.97 

.1511 

0.3450 

24.35 

.1207 

0.2729 

18.55 

.0910 

0  2024 

12  22 

.0587 

0.1294 

9.148 

1  0433 

0.0954 

6.559 

1.0305 

0.0676 

3.540 

1.0159 

0  0360 

5.345 
1.356 

1.0246 
1.0G51 

0.0548 
0.0136 

(Barnes,  J.  Phys.  Chem.  1898,  2.  546.) 
Sp.  gr.  of  HCl+Aq  at  18°/4°. 


g.  HCI  in  100  g.  of  solution 

Sp.  gr. 

0-12149 
O.C60757 
0.040609 
0.030328 

0.99928 
0.99900 
0.9988V 
0  99881 

(Jahn,  Z.  phys.  Ch.  1900,  33.  567.) 

HCI  is  not  absorbed  by  cone.  H2SO4+Aq/ 

but  in  large  amounts  by  anhydrous  H2SO4 

(Aime.) 

Absorption  of  HCI  by  H2SO4+Aq. 

Temp.  =  17°. 

g.  per  1. 

g.  per  100  g. 

Sp.  gr. 

HCI 

H2S04 

HCI 

H2SO4 

1.211 

517.8 

42.7 

1.220 

487.3 

'22^7 

39.9 

Y.86 

1.220 

478.8 

58.0 

39.2 

4.75 

1.235 

455.3 

99.3 

36.9 

8.04 

1.260 

418.0 

161.7 

33.2 

12.8 

1.305 

371.4 

273.2 

28.5 

20.9 

1.355 

306.6 

417.7 

22.6 

30.8 

1.430 

215.3 

638.2 

15.0 

44.6 

1.545 

96.7 

917.6 

6.26 

59.4 

1.580 

51.3 

1033.5 

3.25 

65.4 

1.660 

10.3 

1224.0 

0.62 

73.7 

1.735 

1.89 

1344.9 

0.11 

77.5 

1.815 

1.24 

1615.3 

0.068 

89.0 

CHLORHYDRIC  ACID 


223 


Absorption  of  HC1  by  H2SO4+Aq— Cont. 
Temp.  =  40°. 


gr. 


.185 

.195 

.210 

.255 

.255 

,340 

,400 

,520 

575 

1.650 

1.725 

1.755 

1.770 


ff.  per  1. 


421.4 
416.4 
392.1 
346.3 


325.4 
247.4 
161.6 
50.9 
18.5 
2.9 
1.4 
0.57 
0.52 


H«S04 


42.2 

70.0 

107.7 

211.2 


236.3 

383.7 

619.4 

929.3 

1046.0 

1207.6 

1370.5 

1428.4 

1478.4 


g.  per  100  g 


HC1 


35.6 

34.8 

32.4 

27.6 

25.9 

18.5 

11.5 
3.35 
1.17 
0.17 
0.081 
0.032 
0.029 


H2S04 


3.5 
5.8 
8.9( 
16.8 
18.8 
28.6 
44.2 
61  .'1 
66.4 
73.2 
79.4 
81.4 
83.5 


Temp.  =70°. 


gr. 


145 
150 
160 
180 
225 
230 
315 


1.380 


510 
560 
700 
745 


1.745 


HCl 


374.1 
357.3 
353.8 
341.3 
277.7 
274.3 
173.7 
96.5 
23  6 
8.4 
0.86 
0.62 
0.57 


H2S04 


18.4 

38.9 

55.7 

93.6 

231.9 

246.4 

476.7 

661.8 

946.1 

1055.0 

1371.3 

1448.2 

1455.2 


g.  per  100  g. 


HCl 


32.7 

31.1 

30.5 

28.9 

22.8 

22.3 

13.2 
6.99. 
1.56 
0.54 
0.05 
0.035 
0.032 


H2S04 


1.61 
3.38 
4.80 
7.93 
18.9 
20.0 
36.2 
48.0 
62.7 
67.6 
80  ..7 
83.0 
83.4 


(Coppadoro,  Gazz.  ch.  it.  1910,  39.  II,  626.) 

100  pts.  alcohol  of  36°  B  absorb  68  pts.  HCl 
at  12.5°.  (Boullay.) 

Alcohol  of  0.836  sp.  gr.  dissolves  327  vols. 
HCl  at  17.5°  and  758  mm.  pressure,  and  the 
solution  has  sp.  gr.=  1.005.  (Pierre,  A.  ch.  (3) 
31.  135.) 

Solubility  of  HCl  in  methyl  alcohol  (absolute) 
att°. 


t° 

%  HCl 

t° 

%  HCl 

-10.3 

54.6 

18 

46.9 

0 

51.3 

31.7 

43 

(de  Bruyn,  R.  t.  c.  11.  112.) 

Solubility  of  HCl  in  ethyl  alcohol  (absolute) 
at  t°. 


t° 

%  HCl 

t° 

%HC1 

0 
6.5 
11.5 

45.4 
44.2 
42.7 

19.2 
23.5 
32.0 

41 
40.2 
38.1 

(de  Bruyn,  l.c .) 


Solubility  of  HCl  in  ether  at  t°  and  760  mm. 
pressure. 


t° 

%HC1 

t° 

%  HCl 

—9.2 

37.51 

15 

27.62 

—  5 

37.0 

20 

24.9 

0 

35.6 

25 

22.18 

+  5 

33.1 

30 

19.47 

10 

30.35 

(Schuncke,  Z.  phys.  Ch.  1894,  14.  336.) 

Sol.  in  glacial  HC2H3O2,  ether,  hexane, 
benzene,  xylene,  etc. 

Oil  of  turpentine  absorbs  50%  HCl 
(Thenard.) 

Oil  of  turpentine  absorbs  163  vols.  HCl  at 
22°  and  724  mm.;  isoterebenthene  absorbs 
34%  at  24°  and  724  mm.;  metaterebenthene 
absorbs  17.7%  at  24°  and  724  mm.  (Berthe- 
lot.) 

Oil  of  lavender  absorbs  68.7  vols  at  24° 
(Thfnard.) 

Oil  of  lavender  absorbs  210  vols.  without 
being  saturated;  oil  of  rosemary  absorbs  218 
vols.  at  22°;  sol.  in  0.4  vol.  petroleum. 
(Saussure.) 

Absorbed  by  caprylic  alcohol.    (Bouis.) 

Fuming  HCl-fAq  is  sol.  in  glycerine  and 
miscible  with  cone.  HC2H»O2. 

Solubility  of  HCl  in  phenol  -f-Aq  at  12°. 


Comp.  of  H2O  layer 


HCl 


0 

3.1 

6.6 

8.0 
10.7 


%  phenol 


7.45 
6.6 
5.3 
5.1 

4.8 


Ccmp.  of  phenol  layer 


%  HCl 


0 
0.09 

0.2 

0.36 

0.52 


%  phenol 


72 
7g 
80.3 
82.6 

84.5 


Composition  of  solution  in  contact  with  solid  phenol. 


H2O 


11.22 

14.98 

84.5 

80.38 

72.43 

60.25 


HCl 


0 

C.52 
10.7 
15.64 
24.37 
36.25 


%  phenol 


88.78 

84.5 
4.8 
3.98 
3.2 
3.5 


Schreinemakers,  Z.  phys.  Ch.  1912,  79.  553.) 

+H2O.    F.-pt.-  15.35°. 

Very  sol.  in  H2O  but  only  slightly  sol.  in 
HCl.  (Rupert,  J.  Am.  Chem.  Soc.  1909,  31. 
66.) 

+2H2O.      M.-pt.~17.4c. 

+3H2O.  M.-pt.-24.8°.  (Pickering,  B. 
893,  26.  280.) 

The  composition  of  the  hydrates  formed 
y  HCl  at  different  dilutions  is  calculated 


224 


CHLORHYDRIC  CYANHYDRIC  ACID 


from  determinations  of  the  lowering  of  the 

Solubility  of  Ba(ClO3)2  in  H2O. 

f.-pt.  produced  by  HC1,  and  of  the  conduc- 
tivity and  sp.  gr.  of  HCl+Aq.    (Jones,  Am. 

t° 

g.  Ba(ClO3)2  in 

Sp.  gr. 

Ch.  J.  1905,  34.  323.) 

100  g.  H2O 

Chlorhydric  cyanhydric  acid,  3HC1,  2HCN. 

0 

25.5 

1.195 

Decomp.    by    H2O    or    alcohol;    sol.    in 
HC2H3O2.     Insol.  in  ether,   chloroform,   or 

20 
40 

39.3 
55.9 

1.274 
1.355 

acetic  ether.    (Claisen,  B.  16.  309.) 

60 

74.1 

1  .  433 

HC1,  HCN.    Sol.  in  H2O,  absolute  alcohol, 

80 

92.1 

1.508 

HC2H3O2,   and  CHC13,   with  decomp.;  de- 
comp.  is  especially  rapid  in  H2O.     (Gautier, 

100 
105.6* 

113.2 
120. 

1.580 
1.600 

A.  ch.  (4)  17.  130.) 

*  Rnt.    nf  sfl.f.    anl  lit/inn 

Chloric  acid,  HC1O3. 

Known  only  in  aqueous  solution,  which  can 
be  concentrated  in  vacuo  to  a  sp.  gr.  of  1.282 
at  14.2°,  and  then  contains  40.10%  HC1O3, 
corresponding  to  HC1O3+7H2O;  if  left  longer 
in  vacuo  over  H2SO4  an  acid  corresponding  to 
HC1O3+4KH2O  is  obtained.  Aqueous  solu- 
tion of  HCir3  decomp.  at  40°.  (Kammerer, 
Pogg.  138.  390.) 

Chlorates. 

All  chlorates  except  mercurous  chlorate  are 
sol.  in  H2O;  most  of  them  are  deliquescent; 
many  are  sol.  in  alcohol. 

Aluminum  chlorate,  A1(C103)3+6H2O. 

Very  hygroscopic.  (Dobroserdow,  G.  C. 
1904,  II.  177.) 

+9H2O.  Very  sol.  in  cold  but  much  less 
than  in  hot  H2O.  (Dobroserdow.) 

Ammonium  chlorate,  NH4C1O3. 

Easily  sol.  in  H2O;  less  sol.  in  alcohol. 

Much  less  sol.  in  H2O  at  0°  than  NaC103. 
(Storer.) 

Very  si.  sol.  in  absolute  alcohol.  (Wachter, 
J.  pr.  30.  321.) 

Barium  chlorate,  Ba(ClO3)2-hH2O. 

Sol.  in  4  pts.  cold,  and  less  hot  H20. 
(Chevenix.) 

100  pts.  H2O  dissolve  at: 
0°  20°  40°  60     80°   1CO° 
22.8  37.Q  52.1  77.5  98.0  126.4  pts.  Fa(ClO3)2. 

100  grams  sat.  Ba(ClO3)2+Aq  at  t°  con- 
tain grams  anhydrous  Ba(ClO3)2. 


t° 

Grams 
Ba(C103)2 

t° 

Grams 
Ba(ClO2)a 

Eutectic  point. 
-2.749  ±0.004 
0 
+10 
20 
25 
30 
40 

15.28 
16.90 
21.^3 
25.26 
27.53 
29.43 
33.16 

50 
60 
70 
80 
90 
99.1 
"104.6 

36.69 
40.05 
43.04 
45.90 
48.70 
51.17 
52.67 

*  104.6°  is  bpt.  at  740  mm.  pressure=  105.0° 
at  760  mm.  pressure. 
(Anschutz,  Z.  phys.  Ch.  1906,  56.  238.) 

(Carlson,  Dissert.  1910.) 

Only  slight  traces  dissolve  in  absolute 
alcohol.  (Wachter,  J.  pr.  30.  334.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899,  II. 
1014.) 

Difficultly  sol.  in  acetone.  (Naumann,  B. 
1904,  37.  4328.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethylacet  ate  (Naumann, 
B.  1910,  43.  314.) 

Bismuth  chlorate. 

Known  only  in  solution,  which  decomp.  on 
evaporation. 

Cadmium  chlorate,  Cd(ClO8)2+2H2O. 

Very  deliquescent;  sol.  in  H2O  and  alcohol. 
Melts  in  crystal  H2O  at  80°.  (Wachter,  J.  pr. 
30.321.)  ' 

Solubility  in  H2O. 

Sat.  solution  contains  at: 


-20° 
72.18 

49° 
80.08 


-15° 
72.53 


0° 
74.95 


+  18° 
76.36 


65° 
82.95%  Cd(ClO3)2. 

Sp.  gr.  of  solution  containing  76.36% 
Cd(ClO3)2  at  18°  =2.284.  (Meusser,  B.  1902, 
35.  1422.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

Cadmium     chlorate     ammonia,     Cd(ClO3)2, 
6NH3. 

Ppt.    (Ephraim,  B.  1915,  48.  49.) 

Caesium  chlorate,  CsClO3. 
100  g.  H2O  dissolve  at: 

0°  8°          19.8°         30°         42.2° 

2.46        3.50          6.28        9.53         14.94 

50°  77°  99° 

19.40        41.65        76.5  g.  CsClO3. 
(Calzolari,  Ace.  Sc.  med.  di  Ferrara,  1911, 
85.  150.) 

Calcium  chlorate,  Ca(ClO3)2-f  2H2O. 

Deliquescent;  very  sol.  in  H2O  and  alcohol. 
(Wachter,  J.  pr.  30.  323.) 


CHLORATE,  MAGNESIUM 


225 


Melts  in  its  water  of  crystallization  at  over 
100°. 

Sp.  gr.  of  solution  sat.  at  18°  =  1.729,  con- 
taining 64%  Ca(ClO8)2.  (Mylius  B.  1897, 
30.  1718.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899,  II. 
1014;  Naumann,  B.  1904,  37.  4328.) 

Chromic  chlorate. 

Easily  sol.  in  H2O.  (Prudhomme,  C.  C. 
1890,  1.  668.) 

Cobaltous  chlorate,  Co(ClO3)2+2H2O. 
(Meusser,  B.  1902,  35.  1418.) 
+4H2O.    Solubility  in  H2O. 
Sat.  solution  contains  at: 

•18°      21°      35°      47°      61° 

64.19  64.39  67.09  69.66  76.12%  Co(GlO3)2. 

Sp.  gr.  of  solution  containing  64.19% 
Go(ClO3)2  at  18°  =  1.861.  (Meusser,  B.  1902, 
35.  1418.) 

+6H2O.  Very  deliquescent.  Sol.  in  H2O 
and  alcohol.  Melts  in  crystal  H2O  at  50°. 
(Wachter,  J.  pr.  30.  321.) 

Solubility  in  H2O. 

Sat.  solution  contains  at: 

-21°       -19°         0°      +10.5° 
53.30       53.61       57.45      61.83%  Co(ClO3)2. 
(Meusser,  B.  1902,  35.  1418.) 

Cupric  chlorate,  basic,  Cu(ClO3)2,  3Cu(OH)2. 
Insol.  in  H2O.  Very  sol.  in  dil.  acids.  Sol. 
in  warm  cone.  Cu(ClO3)2+Aq,  the  solubility 
increasing  with  the  cone,  and  temp.  (Bour- 
geois, Bull.  Soc.  1898,  (3)  19.  950.) 

Cupric  chlorate,  Cu(ClO3)2+4H20. 
Solubility  in  H2O. 
Sat.  solution  contains  at: 


-31°         -21° 
54.59         57.12 


+0.8°  18°  45° 

58.51        62.17        66.17 


59.6°          71° 

69.42         76.9%  Cu(ClO3)2. 

Sp.  gr.  of  the  solution  containing  62.17% 
Cu(C108)2  at  18°  =  1.695.  (Meusser,  B.  1902, 
35.  1420.) 

+6H2O.  Very  deliquescent.  Easily  sol. 
in  H2O  and  alcohol.  Melts  in  its  crystal  H2O 
at  65°.  (Wachter,  J.  pr.  30.  321.) 

Sp.  gr.  of  Cu(ClO3)2+Aq  at  15°. 
%Cu(C103)2       2.106          4.778          6.945 
Sp.  gr.  1.01620       1.03857       1.05714 

Cu(ClO3)2       10.016        14.387 
p.  gr.  1.0844       1.12531 

(Traube,  Gm.-K.  6.  1,  921.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 


Cupric  chlorate  ammonia,  Cu(ClO3)2,  4NH3. 

Ppt.    Not  hydroscopic.    Insol.  in  alcohol. 

Cu(ClO3)2,6NH3.  Not  hydroscopic.  (Eph- 
raim,  B.  1915,  48.  46.) 

Erbium  chlorate,  Er(ClO3)3+8H2O. 
Deliquescent.    Sol.  in  H2O  and  alcohol. 

Glucinum  chlorate. 

Known  only  in  aqueous  solution,  which  de- 
composes on  evaporation. 

Ferrous  chlorate. 
Known  only  in  solution. 

Ferric  chlorate,  Fe(ClO3)3. 
Sol.  in  H2O. 
Basic  salt.    Insol.  in  H2O. 

Lanthanum  chlorate,  La(ClO3)3. 
Deliquescent.    (Cleve.) 

Lead  chlorate,  Pb(ClO3)2+H2O. 

Deliquescent;  easily  sol.  in  H2O  and  alcohol. 
(Wachter,  J.  pr.  30.  321.) 

Sp.  gr.  of  solution  sat.  at  18°  =  1.947  and 
contains  60.2%  Pb(ClO3)2.  (Mylius,  B. 
1897,  30.  1718.) 

ICO  g.  H2O  dissolve  440  g.  Pb(ClO8)2  at 
18°;  sp.  gr.  of  sat.  solution  =  1.63.  (Carlson, 
Dissert.  1910.) 

Lithium  chlorate,  LiClO3+^H2O. 

Very  deliquescent  and  sol.  in  H2O.  Very 
easily  sol.  in  alcohol.  Melts  at  50°  in  its 
crystal  water.  (Wachter,  J.  pr.  30.  321.) 

LiClO3+Aq  sat.  at  18°  contains  75.8% 
LiClO3.  Sp.  gr.  =  1.815.  (Mylius,  B.  1897, 
30.  1718.) 

483  g.  LiClOs  dissolve  in  100  g.  H2O  at  15°; 
sp.  gr.  of  solution  =  1.82.  (Carlson,  Dissert. 
1910.) 

Contains  3H2O,  and  is  not  deliquescent. 
(Lagorip,  Zeit.  f.  Kryst.  16.  80.) 

Salt  is  anhydrous.  (Retgers,  Z.  phys.  Ch. 
5.  449.) 

Magnesium  chlorate,  Mg(ClO3)2. 

128.1  g.  Mg(ClO3)  dissolve  in  100  g.  H2O 
at  19°;  sp.  gr.  of  solution  =  1.59.  (Carlson, 
Dissert.  1910.) 

Sp.  gr.  of  solution  containing  56.5% 
Mg(C103)2  at  18°  =  1.564.  (Meusser,  I.e.) 

Sp.  gr.  of  solution  sat.  at  18°  =  1.594,  con- 
taining 56.3%  Mg(ClO3)2.  (Mylius,  B.  1897, 
30.  1718.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014.) 

+2H2O.    Solubility  in  H2O. 

Sat.  solution  contains  at: 

39.5°        61°         68°          93° 
65.37     69.46     70.69     73.71%  Mg(ClO3)2. 
(Meusser,  B.  1902,  36.  1416.) 


226 


CHLORATE,  MANGANOUS 


+4H2O.    Solubility  in  H20. 
Sat.  solution  contains  at: 

42°          65.5° 

63.82        69.12%  Mg(ClO3)2. 
(Meusser,  I.e.) 

+6H2O.  Very  deliquescent  and  sol.  in 
H2O.  Very  easily  sol.  in  alcohol.  Melts  at 
40°  in  its  crystal  water.  (Wachter,  J.  pr.  30. 
325.) 

Solubility  in  H2O. 

Sat.  solution  contains  at: 

-18°    0°      +18°    29°      35° 
51.64  53.27  56.50  60.23  63.65%  Mg(C108)2. 
(Meusser) 

Manganous  chlorate,  Mn(C103)2. 

Known  only  in  solution  which  decomposes 
on  evaporation.  (Wachter.) 

Mercurous  chlorate,  Hg2(ClO3)2. 

o.  Easily  sol.  in  alcohol  and  H20.  (Wach- 
ter, J.  pr.  30.  321.) 

/8.  Insol.  in  H20;  easily  sol.  in  HC2H3O2+ 
Aq.  (Wachter.)  Decomp.  by  boiling  H2O. 

Mercuric  chlorate,  2HgO,  C12O6+H2O. 

Deliquescent.  Decomp.  by  H2O  into  oxide 
and  an  acid  salt.  (Wachter.) 

Sol.  in  4  pts.  cold  H2O.    (Chevenix,  1802.) 

Nickel  chlorate,  Ni(ClO3)2+4H2O. 
Solubility  in  H2O. 
Sat.  solution  contains  at: 

48.5°         55°          65°        79.5° 
67.60      68.78       69.05       75.50%  Ni(ClO,)2. 
(Meusser,  B.  1902,  35.  1419.) 

+6H2O.  Deliquescent.  Easily  sol.  in  H2O 
and  alcohol.  Melts  in  crystal  H2O  at  80°. 
"(Wachter,  J.  pr.  30.  321.) 

Solubility  in  H2O. 

Sat.  solution  contains  at:  '  ;  /•.; 

-18°   -8°       0°      +18°    40° 
49.55  51.52  52.66  56.74  64.47%  Ni(ClO3)2. 

Sp.    gr.    of    solution    containing    56.74% 

Ni(C103)2atl8 

Goes  over  into  4H2O  salt  at  39°.  (Meusser.) 
156  g.  Ni(ClO3)2  dissolve  in  100  g.  H2O  at 

16°;  sp.  gr.  of  solution  =  1.76.    (Carlson,  Dis- 
1910. 


t°                ...      28           3 

5          4.0 
2.3       14.4 

47           65 
18.3      29.1 

Pts.  KClOs   .     .        9.5      1 

(Gerardin.)  ' 
100  pts.  H2O  dissolve  pts.  KClOs  -at  t°. 

t° 

Pts. 
KC1O3 

t 

Pts. 
KClOs 

12.05 
18.96 
35.40 
60  .  24      ' 

0 
13.32 
15.37 
24.43 

3.33 
5.60 
6.03 

8.41 

35.0 
49.08 

74.89 
104  .  78 

(Gay-Lussac,  A.  ch.  11.  314.) 

100  pts.  H2O  dissolve  pts.  KC1O3  at  t°. 

t° 

Pts. 
KClOs 

t° 

Pts. 
KClOs 

0 
100 

3.3 
56.5 

130 
180 

88.5 
190 

sert. 


.) 


JNickel  chlorate  ammonia,  Ni(ClO3)2,  6NH3. 
Ppt.    (Ephraim,  B.  1915,  48.  47.) 

Potassium  chlorate,  KC1O3. 

Sol.  in  H2O  with  absorption  of  heat. 

Sol.  in  about  16  pts.  cold,  and  in  much  less  hot  H2O 
(Chevenix,  1802.) 

Sol.  in  30.03  pts.  H2O  at  0°;  17.85  pts.  at  13.3°;  and 
n  1.66  pts.  .at  104.78°.  ,  (M.  R.  and  P,  .) 


Sol.  in  16  pts.  H2O  at  18.75°.     (Abl.) 
100  pts.  HsO  at  15.5°  dissolve  6.2  pts.;  at  100°,  40 
pts.  (Ure's  Diet.) 


100  pts.  H2O  dissolve  pts.  KClOs  at  t°- 


(Tilden  and  Shenstone,  Roy.  Soc.  Proc.  35. 
345.) 

100  pts.  H2O  dissolve  pts.  KC1O3  at  t°. 


t° 

Pts. 
KClOs 

t° 

Pts. 
KClOs 

120 
136 

73.7 
98.9 

160 
190 

148 
183 

(Tilden  and  Shenstone,  Phil.  Trans.  1884.  23.) 

Coefficient  of  solubility  is  3.2+0.109t+ 
0.0043t2  between  0°  and  35°.  (Blarez,  C.  R. 
112.  1213.) 

Sat.  KClO3+Aq  contains  %  KC103  at  t°. 


t 

%  KClOs 

t° 

%  KClOs 

-0.5 

2.6 

92 

31.2 

-0.3 

2.4 

106 

37.2 

+4.5 

3.5 

130 

47.0 

4.5 

2.9 

171 

,  59.8 

11 

4.7 

180 

62.1 

19 

6.1 

190 

63.1 

29 

8.9 

200 

64.2 

36 

9.9 

207 

66.0 

42 

11.4 

300 

87.0 

56 

15.1 

330 

96.7 

58 

16.6 

'    Cfitard,  A.  ch.  1894,  (7)  2.  528.) 

CHLORATE,  MANGANOUS 


227 


Solubility  in  H2O. 


Temp. 

%  KC103 
in  a  sat.  sol. 

Pts.  sol.  in 
100  pts.  H2O 

Pts.  H2O  to 
1  pt.  KClOs 

0° 

3  06 

3.14 

31.8 

5 

3.67 

3.82 

26.2 

10 

4.27 

4.45 

22.5 

15 

5.11 

5.35 

18.5 

20 

6.76 

7.22 

13.6 

25 

7.56 

8.17 

12.2 

30 

8.46 

9.26 

10.8 

35 

10.29 

11.47 

8.7 

40 

11.75 

13.31 

7.5 

45 

13.16 

14.97 

6.6 

50 

15.18 

17.95 

5.6 

55 

16  85 

20.27 

4.9 

60 

18.97 

23.42 

4.2 

65 

20.32 

25.50 

3.9 

70 

22.55 

29.16 

3.4 

75 

24.82 

32.99 

30 

80 

26.97 

36.93 

2.6 

85 

29.25 

41.35 

2.4 

90 

31.36 

46.11 

2.1 

95 

33.76 

.    51.39 

1.9 

100 

35.83 

55.54 

1.8 

(Pawlewski,  B.  1899,  32.  1041.) 

1  1.  KClO3+Aq  at  25°  contains  675  milli- 
mols.  KC103.  (Calvert,  Z.  phys.  Ch.  1901, 
38.  541.) 

100  g.  H2O  dissolve  at: 

0°         20°        40°         60° 
3.3        7.4        13.8        24.0  g.  KC1O3 
Sp.  gr.  1.021     1.045      1.073      1.115 

80°  100°        104°  * 

37.7          56.5          59.9g.KC103, 
Sp.gr.  1.165         1.219         1.230 

*  Bpt.  of  sat.  solution. 

(Carlson,  Dissert.  1910.) 

100  g.  H2O  dissolve  at: 

8°     19.8°       30°        99° 
4.48      7.15     10.27    57.3  g.  KC1O3. 
(Calzolari,  Ace.  Sc.  med.  di  Ferrara, 
1911,  85.  150.) 

Sat.  KClO3+Aq  contains  at: 
53°        68°        81°        86°(?) 
17.37    23.25    23.53    30.46%  KC1O3. 
(Tschugaeff,  Z.  anorg.  1914,  86.  161.) 

Sp.  gr.  of  KClO3+Aq,  according  to  Kremer's 
experiments  (Pogg.  96. 62),  and  Gerlach's 
calculations.  (Z.  anal.  8.  290.) 


%  KClOs 

Sp.  gr. 

%  KClOs 

Sp.  gr. 

1 

1.007 

6 

1.039 

:    2 

1.014 

7 

1.045 

3 

1.020 

8 

1.052 

4 

1.026 

9 

1.059 

5 

1.033 

10 

1.066 

Sp.  gr.  of  KC103+Aq  at  20°  containing  1 
mol.  KC1O3  to  100  mols.  H2O  =  1.04122. 
(Nicol,  Phil.  Mag.  (5)  16.  122.) 

Sp.  gr.  of  KClOs+Aq  at  15°  containing  5% 
KC1O3  =  1.0316.  (Kohlrausch,  W.  Ann.  1879. 
1.) 

B.-pt.  of  KClOa+Aq  containing  pts.  KC1O3 
.;.'•>:       to  100  pts.  H2O. 


Pts. 
KClOs 

B.-pt, 

Pts. 
KClOa 

B.-pt. 

6.5 
13.2 
20.2 

27.8 
35.8 

100.5° 
101.0 
101.5 
102.0 
102.5 

44.6 
53.4 

62.2 
69.2 

103.0° 
103.5 
104.0 
104.4 

(Gerlach,  Z.  anal.  26.  450.) 

Saturated  solution  boils  at  105°.  (Kremers.) 

Saturated  solution  boils  at  104.2°,  and  con- 
tains 61.5  pts.  KC1O3  to  100  pts.  H2O. 
(Legrand.) 

Saturated  solution  boils  at  103.3°,  and  con- 
tains 66.6  pts.  KC103  to  100  pts.  H2O.  (Grif- 
fiths.) 

Saturated  solution  boils  at  104.4°.  (Ger- 
lach, Z.  anal.  26.  427.) 

Sol.  in  pure  HNO3  without  decomp.,  but 
decomp.  at  once  by  HNO3  containing  NO2. 
(Millon,  A.  ch.  (3)  6.  92.) 

Sol.  in  sat.  NH4Cl+Aq  without  causing 
pptn. 

1  mol.  ( =  129  pts.)  KC1O3  dissolves  in  2493 
vols.  H2O;  in  2208  vols.  H2O  when  1  mol. 
(  =  59  pts.)  NaCl  is  added;  in  2060  vols.  H2O 
with  2  mols.  ( =  118  pts.)  NaCl;  and  in  1910 
vols.  H2O  with  4  mols.  (=236  pts.)  NaCl. 
(Gladstone,  Chem.  Soc.  16.  302.) 

KC1O3  is  sol.  in  about — 

29.50  pts.  H2O. 

35.50  pts.  NH4OH+Aq  cone.      . 

39.00  pts.  dil.  NH4OH+Aq  (1  vol.  cone.:  3 
vols.  H2O). 

30.50  pts.  HNOa+Aq  (1  vol.  cone.  HNO3: 
5  vols.  H2O). 

33.0  pts.  HCl+Aq  (1  vol.  cone.  HC1: 4  vols. 
H20). 

48.00  pts.  HC2H3O2+Aq  (1  vol.  commer- 
cial HC2H3O2:1  vol.  H20). 

31.50  pts.  NH4Cl+Aq  (1  pt.  NH4C1:10  pts. 
H2O). 

18.00  pts.  NH4NO3+Aq  (1  pt.  NH4NO3:10 
pts.  H2O). 

34.00  pts.  NH4C2H302+Aq  (dil.  NH4OH  + 
Aq+dil.  HC2H802+Aq). 

32.50  pts.  NaC2H3O2-f-Aq  (commercial 
HC2H3O2+Na2CO3,  diluted  with  4  vols.  H2O). 

31.50  pts.  Cu(CjH|Oi)«+Aq.  (See  Stolba, 
Z.  anal.  2.  390.) 

33.50  pts.  cane-sugar  (1  pt.  cane-sugar  :  10 
pts.  H2O). 

36.50  pts.  grape-sugar  (1  pt.  grape-sugar:  10 
pts.  H2O).  (Pearson,  Zeit.  Chem.  1869.  662.) 

Addition  of  K  salts  to  sat.  KClO3-f-Aq  ppts. 
KC1O3  in  such  a  way,  that  the  sum  of  the 


228 


CHLORATE,  MANGANOUS 


KC103  remaining  in  solution  and  the  K  in  the 
salt  added,  is  a  constant,  which  constant  is 
equal  to  the  solubility  of  KC1O3,  so  that  the 
following  formula  represents  the  coefficiency 
of  solubility  of  KC1O3  after  addition  of  a  K 
salt,  3.2+0.109t+0.0043t2-K  of  salt  added. 
(Blarez,  C.  R.  112.  1213.) 

Solubility  of  KC1O3+T1C1O3. 

Solubility  in  KOH+Aq  at  25 

o 

KOH  +Aq 

Millimols  KClOs  per  litre 
of  the  solulion 

Vs-normal 
^-normal 

624 
573 

(Calvert,  Z.  phys.  Ch.  1901,  38.  541.) 
Solubility  in  H2O2  at  25°. 

100  g.  H2O  dissolve  g.  salts 

t° 

g.  TIClOs 

g.  KClOs 

Concentration  of  H2C>2 
millimols  per  litre 

Millimols  KClOa  per  litre 
of  the  solution 

0 
15 
50 
100 

2.8 
10 
12.67 
57.3 

3.3 
1.5 
16.2 

48.2 

1260 
1310 

730 
737 

(Calvert,  I.e.) 

Solubility  in  l/±  normal  KOH+Aq 
iD  presence  of  H2O2  at  25°. 

(Rabe,  Z.  anorg.  1902,  31.  156.) 
Solubility  of  KC1O3  in  KNO3+Aq. 

t° 

g.  per  1. 

Concentration  of  EbOz 
millimols  per  litre 

Millimois  KClOs  per  lit.re 
of  the  solution 

KNO3                       KC103 

15 
276 
954 
1073 

578 
584 
616 
673 

19.85 

0.00                 69.88 
12.65                 64.86 
25.29                 60.33 
101.19                 45.85 
202.38                 40.20 

(Calvert,  I.e.) 

Moderately  sol.  in  liquid  NH3.    (Franklin. 
Am.  Ch.  J.  1898,  20.  828.) 
Neither  dissolved  nor  attacked  by  liquid 
NO2.  (Frankland,  Chem.  Soc.  1901,  79.  1361.) 
Sol.  in  120  pts.  alcohol  of  83%  at  16°. 
(Wittstein.) 
Sol.  in  120  pts.  alcohol  of  77.1%.     (Pohl, 
W.  A.  B.  6.  595.) 
Insol.  in  absolute  alcohol.     (Gerardin.) 

Solubility  of  KC1O3  in  dil.  alcohol.    D  =  sp. 
gr.  of  alcohol;  S  =  solubility  in  100  pts. 
alcohol  at  t°. 

23.87 

0.00                 79.09 
50.59                 63.14 

(Arrhenius,  Z.  phys.  Ch.  1893,  11.  397.) 
Solubility  in  KCl+Aq  at  20°  C. 

G.  KCl  in 
1  litre 

G.  KC103 
in  1  litre 

Sp.  gr. 

0 
10 
20 
30 
40 
50 
60 
70 
80 
90 
100 
110 
120 
130 
140 
150 
160 
170 
180 
190 
200 
210 
220 
230 
240 
250 

71.1 
58 
49 
43 
39.5 
36.5 
34 
32 
30 
28 
27 
25.5 
24.5 
23.5 
22.5 
21.5 
21.0 
20.5 
20.0 
20.0 
20 
20 
20 
20 
20 
20 

1.050 
.050 
.050 
.050 
.054 
.058 
.064 
.070 
.075 
.081 
.086 
.091 
.098 
1.103 
1.108 
1.113 
1.119 
1.124 
1.130 
1.135 
1.140 
1.145 
1.150 
1.156 
1.161 
1.168 

D  =0.9904 

D  =0.9848 

D  =0.9793 

t° 

s 

49 
63 
75 
9.1 
10.2 
13.6 
16.2 

t° 

14 
26 
39 
47 
55 
65 
66 

s 

4.7 
7.1 
9.3 
12.8 
16.1 
22.3 
22.5 

t 

g 

13 
21 
25 
30 
35 
44 
50 

14 
26 
38 
46 
51 
63 
65 

3.2 
5.4 
7.9 
10.8 
12.2 
17.5 
19.0 

D  =0.9726 

D  =0.9573 

D  =0.9390 

t° 

s 

t° 

s 

t° 

s 

13 
20 
33 
43 
56 
59 

2.2 
3.3 

5.8 
7.2 
11.4 
12.9 

13 
20 
29 
36 
55 
60 
63 

1.9 

2.7 
3  6 
4.3 
7.9 
9.7 
10.5 

14.5 
28 
40 
50 
62 
67 

1.1 
2.2 
3.4 
4.3 
6.6 
7.6 

(Winteler,  Z.  Elektrochem.  1900,  7.  361.) 

CHLORATE,  SODIUM 


229 


Solubility  of  KCIO3  in  dil.  alcohol  —  -Continued. 

Potassium  silver  chlorate,  KC1O3,  AgClO3. 

D  =0.9111 

D  = 

=0.8967                D  =0.8429 

(Pfaundler,  W.  A.  B.  46,  2.  266.) 

t 

s 

t° 

S                 t° 

s 

Rubidium  chlorate,  RbClO3. 

13 
25 
32 
52 

0.74 
1.08 

1.78 
3.35 

12 
31 
43 

58 

6.46        25 
1.28        34 
1.95        56 
3.10        64 

0.09 
0.12 
0.24 
0.32 

100  pts.  H2O  dissolve  2.8  pts.  at  4.7°;  3.9 
pts.  at  13°;  4.9  pts.  at  18.2°;  5.1  pts.  at  19°. 
(Reissig,  A.  127.  33.) 
100  g.  H2O  dissolve  3.1  RbClO8  at  15°; 
sp.  gr.  of  solution  =  1.07.    (Carlson,  Dissert. 

(Gerardin,  A. 

ch.  (4)  6.  148.) 

1910.) 

100  g.  H2O  dissolve  at: 

Solubility 

of  KC1O3  in  alcohol  +Aq. 

0°         8°       19.8°       30° 

wt.  %  alcohol 

g.  KC1O3  per  100  g.  solution 

2.138      3.07      5.36      8.00  g.  RbClO8, 

t=30° 

t=40° 

42.2°       50°        76°        99° 

12.48     15.98    34.12    62.8  g.  RbClO3. 

0 
5 

9.23 

7.72 

12.23 
10.48 

(Calzolari,  Ace.  Sc.  med.  di  Ferrara,  1911,  86. 

10 

6.44 

8.84 

; 

2 

n 

4.51 

6.4C 

V 

30 

3.21 

4^67 

Scandium  chlorate. 

40 

2.35 

3.41 

(Crookes,  Roy.  Soc.  Proc.  1908,  80.  A,  518.) 

50 

1.64 

2.41 

60 

1.01 

4.41 

Silver  chlorate,  AgClO3. 

70 
80 
90 

0.54 
0.24 
G.06 

0.78 
0.34 
0.12 

Sol.  in  10-12  pts.  cold  H2O  (Vauquelin); 
in  8-10  pts.  cold,  and  2  pts.  hot  H2O  (Chev- 
enix); in  5  pts.  cold  H2O  (Wachter).    SI.  sol. 
in  alcohol  (Chevenix);  easily  sol.  in  alcohol 
(Wachter). 

•  (Taylor,  J.  phys.  Ch.  1897,  1.  301.) 

Insol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1370.) 

Very  si.  sol.  in  acetone.  (Krug  and  M'El- 
roy,  J.  Anal.  Ch.  6.  184.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Solubility  of  KC103  in  acetone +Aq. 


wt.  %  acetone 

g.  KClOs  per  100  g.  solution 

t  =30° 

t  =40°      ' 

0 

9.23 

12.23 

5 

8.32 

11.10 

9.09 

7.63 

10.28 

20 

6.09 

8.27 

30 

4.93 

6.69 

40 

3.90 

5.36 

50 

2.90 

4.03 

60 

2.03 

2.86 

70 

1.24 

1.68 

80 

0.57 

0.79 

90 

0.18 

0.24 

(Taylor,  J.  phys.  Ch.  1897,  1.  301.) 

Insol.  in  methyl  acetate.  (Naumann,  B 
1909,  42.  3790);  ethyl  acetate.  (Naumann 
B.  1904,  37.  3601.) 

Solubility  in  glycol  =  0.9%  at  ord.  temp 
(de  Coninck,  Belg.  Acad.  Bull.  1905.  359  ) 

100  g.  glycerol  (sp.  gr.  1.256)  dissolve  3.54  g 
KC1O3  at  15-16°.  (Ossendowski,  Pharm.  J 
1907,  79.  575.) 


Silver  chlorate  ammonia,  AgClO3,  2NH3. 

Easily  sol.  in  H2O  or  alcohol.     (Wachter, 
1843.) 

Sodium  chlorate,  NaC103. 
Deliquescent. 

Sol.   in  3  pts.  cold    and  less  hot  H2O.     (Wachter; 
Chevenix.) 

Sol.  in  3  pts.  H20  at  18.75°.     (Abl.) 

100  pts.  H2O  dissolve  35.5  pts.  NaClOs.   (Ure's  Diet.) 

100  pts.  H2O  dissolve  at: 
0°      20°     40°        60° 
81.9    99     123.5     147.1  pts.  NaC103, 

80°       100°      120° 
175.6    232.6    333.3  pts.  NaClO3. 
(Kremers,  Pogg.  97.  4.) 

100  pts.  H2O  dissolve  89.3  pts.  NaClO3  at 
12C.    (Schlosing.) 

ICO  g.  H2O  dissolve  at: 

-15°    0°       20°  40° 

72       79      101  126    pts.  NaClO3, 

Sp.gr.  1.380  1.389  1.430  1.472 

60°      80°     100°  122°* 
155      189      230       286  pts.  NaClO3. 
Sp.gr.  1.514  1.559  1.604  1.654 
*  Bpt.  of  sat.  solution. 

(Carlson,  Dissert.  1910.) 


230 


CHLORATE,  SODIUM 


100  g.  NaC103+Aq  contain  at: 
4.78°  19.85°  30.05°  35.10°  44.72° 
45.47    48.91    51.22    52.36    54.50  g.  NaClO3. 
(Le  Blanc  and  Schmandt,  Z.  phys.  Ch.  1911, 
77.  614.) 

Sp.  gr.  of  NaClO3+Aq,  containing: 
10       15       20       25       30       25%  NaClO3. 
1.070  1.108  1.147   1.190  1.235  1.282 
(Gerlach,  Z.  anal.  8.  290.) 

Sp.  gr.  of  NaClOs+Aq  at  20°  containing  1 
mol.  NaClO3  in  100  mols.  H2O  =  1.03844. 
(Nicol,  Phil.  Mag.  (5)  16.  122.) 

NaClO3+Aq  containing  7.23%  NaClO, 
has  sp.  gr.  20° /20°  =  1.0496.  (Le  Blanc  and 
Rohland,  Z.  phys.  Ch.  1896,  19.  278.) 

Sat.  solution  boils  at  132°,  and  temp,  can 
be  raised  to  135°  by  supersaturation.  (Krem- 
ers,  Pogg.  97.  4.; 

Easily  sol.  in  liquid  HF.  (Franklin,  Z. 
anorg.  1905,  46.  2.) 

NaClOa+NaCl. 

100  pts.  H2O  dissolve  50.75  pts.  NaClO3  + 
24.4  pts.  NaCl  at  12°;  ICO  pts.  H2O  dissolve 
249.6  pts.NaC103+11.5  pts.  NaCl  at  122°, 
and  when  cooled  to  12°  contain  68.6  pts. 
NaClO3+11.5  pts.  NaCl.  (Schlosing,  C.  R. 
73.  1272.) 

Solubility  in  NaCl+Aq  at  20°  C. 


G.  NaCl 
in  1  litre 

G.  NaClOs 
in  1  litre 

Sp.  gr. 

5 

668 

1.426 

10 

661 

1.424 

15 

653 

1  423 

20 

645 

1.421 

25 

638 

1.419 

30 

630 

1.418 

35 

622 

1.417 

40 

615 

1.415 

45 

607 

1.414 

50 

599 

1.412 

55 

590 

1.411 

60 

582 

1.409 

65 

574 

1.408 

70 

566 

1.406 

75 

559 

1.405 

80 

551 

1.404 

85 

544 

.402 

90 

537 

.401 

95 

529 

.399 

100 

522 

.398 

105 

514 

.396 

110 

507 

.394 

115 

499 

.392 

120 

491 

.391 

125 

484 

.389 

130 

476 

.387 

135 

467 

.385 

140 

459 

.383 

145 

451 

.381 

Solubility  in  NaCl+Aq  at  20°  C.— Continued 


G.  NaCl 
in  1  litre 

G.  NaClOs 
in  1  litre 

Sp.  gr. 

150 

442 

1.379 

155 

432 

1.377 

16C 

423 

1.374 

165 

414 

1.372 

170 

403 

1.369 

175 

393 

1.365 

180 

382 

1.362 

185 

371 

1.359 

190 

360 

1.355 

195 

349 

1.350 

200 

338 

1.345 

205 

326 

1.340 

210 

315 

1.335 

215 

302 

1.330 

220 

287 

1.324 

225 

271 

1.319 

230 

257 

1.313 

235 

243 

1.307 

240 

228 

1.301 

245 

211 

1.295 

250 

197 

1.289 

255  ' 

184 

1.283 

26C 

170 

1.276 

265 

150 

1.270 

270 

135 

1.263 

275 

120 

1.256 

280 

105 

1.249 

285 

91 

1.241 

290 

78 

1.235 

295 

67 

1.226 

300 

55 

1.217 

(Winteler,  Z.  Elektrochem.  1900,  7.  361.) 

Very  sol.  in  liquid  NH3.  (Franklin,  Am* 
Ch.  J.  1898,  20.  829.) 

Sol.  in  34  pts.  alcohol  of  83%  at  16°  and  in 
less  hot  alcohol.  (Wittstein.) 

Somewhat  more  easily  sol.  in  alcohol  than 
NaCl.  (Berzelius.) 

Solubility  of  NaClO3  in  alcohol. 
(g.  NaClO3  per  1.  of  solution.) 


t° 

Alcohol 

90  % 

75% 

50  % 

20 
40 
60 
70 

16.1 
22.9 
29.0 

110.8 
133.5 
155.8 
161.3 

311.3 
321.8 
326.8 

(Carlson,  Dissert.  1910.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

100  g.  glycerol  dissolve  20  g.  NaClO3  at 
15.5°.  (Ossendowski,  Pharm.  J.  1907,  79. 
575.) 


CHLORINE 


231 


Strontium  chlorate,  Sr(ClO3)2+5H2O. 

Very  deliquescent,  and  sol.  in  H20.  (Top- 
soe,  W.  A.  B.  66,  2.  29.) 

Sp.  gr.  of  solution  sat.  at  18°  containing 
63.3%  Sr  (C1O3)2  =  1.839.  (Mylius,  B.  1897, 
30.  1718.) 

Easily  sol.  in  H2O,  less  in  alcohol,  but  more 
sol.  in  alcohol  than  SrCl2.  (Souchav,  A.  102. 
381.) 

Insol.  in  absolute  alcohol.    (Wachter.) 

Thallous  chlorate,  T1C1O3. 

Sol.  in  H2O,  but  decomp.  by  heating. 

100  pts.  H2O  dissolve  at: 
0°     20°     50°      80°     100° 
2.80  3.92  12.67  36.65  57.31  pts.  T1C1O3. 
(Muir,  Chem.  Soc.  29.  857.) 

1 1.  TIClOg+Aq  sat.  at  10°  contains  25.637 
g.  T1C103.  (Roozeboom,  Z.  phys.  Ch.  8.  532.) 

1  1.  H2O  dissolves  0.134  equivalents 
TICK)  3  at  20°;  or  38.51  g.  in  1  1.  of  the  solu- 
tion (mean  of  10  experiments).  (Noyes  and 
Farrell,  J.  Am.  Chem.  Soc.  1911,  33.  1657.) 


Solubility  in  Tl2SO4+Aq  at  20°. 


G.  equiv.  per  1. 

Solid  phase 

TIClOs 

T12S04 

0.1058 

0.1366 

T1C1O3+T12SO4 

(Noyes  and  Farrell,  I.e.) 

Thallic  chlorate,  T1(C103)3+4H2O. 

Very  deliquescent;  sol.  in  H2O.  Decomp. 
slowly  in  the  air.  (Gewecke,  Z.  anorg.  1912, 
76.  273.) 

Ytterbium  chlorate. 

Sol.  inH2O.    (Popp,  A.  131.  179.) 

Yttrium  chlorate,  Y(C1O3)3+8H2O. 

Deliquescent.    Easily  sol.  in  alcohol.    SI. 
sol.  in  ether.    (Cleve.) 

Zinc  chlorate,  Zn(ClO3)2+4H2O. 
Solubility  in  H2O. 
Sat.  solution  contains  at: 


+18° 
66.52 


30° 
67.66 

of 


40° 
69.06 


55C 


75.44%  Zn(ClO3)2. 
solution    containing    66.52% 


Sp.    gr. 
Zn(ClO3)2at  18°  =  1.916. 

(Meusser,  B.  1902,  35.  1417.) 

More  sol.  in  H2O  than  chlorates  of  Mg,  Co, 
Ni  or  Cu;  less  sol.  than  chlorate  of  Cd;  more 
sol.  than  Zn(N03)2.  (Meusser,  I.e.) 

+6H2O.  Very  deliquescent.  Easily  sol.  iD 
H2O  and  alcohol.  Melts  in  crystal  H2O  at  60°. 
(Vauquelin,  A.  ch.  95.  113.) 


Solubility  in  H2O. 

Sat.  solution  contains  at: 


-18° 
55.62 


0° 
59.19 


8°  15° 

60.20      67.32%  Zn(ClO3)2. 
(Meusser,  I.e.) 


Sp.  gr.  of  solution  sat.  at  18°  containing 
65%  Zn(ClO3)2  =  1.914.  (Mylius,  B.  1897, 
30.  1718.) 

Zinc  chlorate  ammonia,  Zr(ClO3)2,  4NH3. 

Zn(ClO3)2,  6NH3.  Ppt.  (Ephraim,  B. 
1915,  48.  48.) 

Perchloric  acid 
See  Perchloric  acid. 

Chlorides. 

Most  chlorides  are  sol.  in  H2O;  a  few,  how- 
ever, are  insol.  or  nearly  so  therein,  the  chief 
of  which  are  AgCl,  Hg?Cl2,  Cu2Cl2,  PtCl2,  and 
AuCl.  Several  chlorides  are  decomp.  into 
insol.  basic  salts  or  hydroxides,  either  by  the 
addition  of  H2O,  as  in  the  case  of  BiCl3  and 
SbCl3,  or  on  evaporating  the  aqueous  solution, 
as  A1C13,  ZnCl2,  MgCl2,  etc. 

Some  chlorides  are  sol.  in  alcohol  or  ether. 

See  under  each  element. 

Chlorine,  C12. 

The  maximum  solubility  of  Cl  in  H2O  is  at 
1C0  (Schonfeld);  at  8-10°  (Gay-Lussac)  ;  at 
9-10°  (Pelouze). 

Solubility  decreases  from  9-0°;  at  100°  the 
solubility  =0.  (Gay-Lussac.) 

Cl2+Aq  sat,  at  6°  has  sp.  gr.  =  1.003.  (Ber- 
thelot.) 

1  vol.  H2O  at  t°  absorbs  vols.  Cl  reduced  to 
0°  and  760  mm.  pressure. 


t° 

Vols.  Cl 

t° 

Vols.  Cl 

10 

2.5852 

26 

1.9099 

11 

2.5413 

27 

1.8695 

12 

2.4977 

28 

.8295 

13 

2.4543 

29 

.7895 

14 

2.4111 

30 

.7499 

15 

2.3681 

31 

.7104 

16 

2.3253 

32 

.6712 

17 

2.2828 

33 

.6322 

18 

2.2405 

34 

.5934 

19 

2.1984 

35 

1.5550 

20 

2.1565 

36 

1,5166 

21 

2  1148 

37 

1.4785 

22 

2.0734 

38 

1.4406 

23 

2.0322 

39 

1.4029 

24 

1.9912 

40 

1.3655 

25 

1.9504 

(Schonfeld, 

A.  93.  26 

.) 

232 


CHLORINE 


Ivol 

.  H2O  absorbs  vols.  Cl  at  t°  (not 
corrected). 

Solubility  of  C12  in  H2O. 
pi  =  Vol.  of  Cl  (reduced  to  0°  and  760  mm.) 
absorbed  by  1  vol.  H2O  under  a  total  pressure 
of  760  mm. 
q=g.  C12  absorbed  by  100  g.  H2O  under  a 
total  pressure  of  760  mm. 

Vols.  Cl 

t° 

Vols.  Cl 

t° 

Vols.  Cl 

tc 

1. 

1. 
2. 

2. 

43 
52 
08 
17 

0 
3 
6.5 

7 

3 
3 
2 
1 

.04 
.00 
37 
.61 

8 
10 
17 
35 

1.19 
0.71 
0.15 

50 
70 
100 

t° 

Pl 

q 

t° 

0l 

q 

10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 

3.095 
2.996 
2.900 
2.808 
2.720 
2.635 
2.553 
2.474 
2.399 
2.328 
2.260 
2.200 
2.143 
2.087 
2.035 

0.980 
948 
918 
889 
861 
835 
809 
784 
760 
738 
716 
698 
680 
662 
646 

25 
26 
27 
28 
29 
30 
35 
40 
45 
50 
60 
70 
80 
90 
100 

.985 
.937 
.891 
.848 
.808 
.769 
.575 
.414 
1.300 
1.204 
1.006 
0.848 
0.672 
0.380 
0.000 

0.630 
615 
600 
587 
574 
562 
501 
451 
415 
386 
324 
274 
219 
125 
000 

(Gay-Lussac,  A.  ch.  (3)  7.  124.) 

1  vol.  H2O  at  8°  absorbs  3.04  vols.  Cl,  which  is  the 
maximum  of  solubility.    At  50°,  1.09  vols.  are  absorbed  ; 
and  at  0°,  1.5  vols.    (Pelouze  and  Fremy.) 

1  vol.  EbO  at  t°  dissolves  vols.  Cl  (not  corrected)  . 

t° 

Vols.  Cl 

t 

Vols.  Cl 

t° 

Vols.  Cl 

0 
9 
10 

1.75-1.80 
2.70-2.75 
2.70-2.75 

12 
14 
30 

2  .  50-2  .  60 
2.45-2.50 
2  .  00-2  .  10 

40 
50 
70 

1  .  55-1  .  60 
1.15-1.20 
0.60-0.65 

(Pelouze,  A.  ch.  (3)  7.  188.) 


1  vol.  H2O  absorbs  vols.  Cl  at  t°. 


t° 

Vols.  Cl 

t° 

Vols.  Cl 

t° 

Vols.  Cl 

0 
5 

8 

1.5  -1.6 
2.05-2.1 
2.5  -2.6 

9 
10 
12 

2.65-2.70 
2.9  -3.0 
2.65-2.75 

14 
16 
30 

2.6  -2.65 
2.35-2.4 
1.8  -1.85 

(Riegel  and  Walz,  Berz.  J.  B.  1846.  72.) 


Solubility  in  H2O  :  a  =  coefficient  of  solubility. 


t° 

a 

t° 

a 

t° 

a 

6.9 

8.4 
9.3 

2.2931 
2.5469 
2.7135 

10.1 
11.2 
13.7 

2.8741 
2.7267 
2.5079 

21.7 
32.1 
36.7 

2.0422 
1.5766 
1.3802 

(Goodwin,  B.  16.  3040.) 


Goodwin  also  gives  tables  for  solubility  of 
Cl  in  HC1  and  various  chlorides,  but  they  do 
not  show  eviden ce  of  accurate  work.  ( A.M  .C . ) 


Cl2+Aq  contains  at  760  mm.  pressure: 

1.44%  Cl  at  0° 
1.07%  "  "  6° 
0.95%  "  "  9° 
0.87%  "  "  12° 


(Roozeboom,  R.  t.  c.  1884,  3.  29.) 
See  also  C12+8H2O. 


(Winkler,  Landolt  and  Bornstein,  Tab.  4th 
Ed.  1912,  597.) 

1  1.  HCl+Aq  (38%  HC1)  dissolves  17.3  g. 
Cl;  1  1.  HCl+Aq  (33%  HC1)  dissolves  11  g. 
Cl;  1  1.  HCl+Aq  (3%  HC1)  dissolves  6.5  g. 
Cl.  (Berthelot,  C.  R.  91.  191.) 


Solubility  of  C12  in  HCl+Aq  at  20-21C 
759-761  mm.  pressure. 


and 


g.  HC1  per  1. 

g.  C12  per  1. 

Coefficient 
of 
absorption 

Solubility 

0 

7.23 

2.1157 

2.2799 

3.134 

5.30 

1.5496 

.6698 

6.248 

4.94 

.4483 

.5607 

9.402 

4.76 

.3942 

.5013 

12.540 

4.85 

.4200 

.5292 

15.670 

5.10 

.4933 

.6092 

31.340 

5.81 

.6736 

.8033 

62.680 

6.38 

.8682 

2.0131 

94.020 

7.19 

2.1044 

2.2677 

125.360 

7.76 

2.2711 

2.4473 

156.700 

8.58 

2.5095 

2.7043 

188.040 

9.23 

2.7020 

2.9117 

219.380 

9.93 

2.9243 

3.1312 

250.720 

10.68 

3.1272 

3.3677 

282.060 

11.87 

3.3278 

3.5859 

313.401 

12.03 

3.5492 

3.8224 

(Mellor,  Chem.  Soc.  1901,  75.  227.) 

Solubility  of  Cl  in  NaCl+Aq.    a  =  coefficient 

of  solubility. 

NaCl  =  9.97%. 


t 

a 

t° 

a 

7.9 
11.9 
15.4 

1.8115 
1.5879 
1.3684 

18.8 
22.6 

1.2785 
1.0081 

CHLORINE  OXIDE 


233 


Solubility  of  Cl  in  NaCl+Aq.—  Continued 
NaCl  =  16.01%. 

Coefficient  of  solubility  of  C12  in  organic 
liquids  at  15°. 

Substance                     Coefficient  of  Solubility 

t 

a 

t 

a 

Carbon  tetrachloride                    51  .  7 
Acetic  anhydride                           39  .  6 
Acetic  acid  (99.84%)                    36  .  7 
"        (90vol.  %)                25.3 
(75vol.  %)                 16.43 
(65vol.  %)                 13.43 

6 
11.6 
16.4 

1.5866 
1.2227 
1.0121 

21 

26 

.4 
.9 

0.8732 
0.7017 

NaCl  =  l9.66%. 

(Jones,  Chem.  Soc.  1911,  99.  392.) 

+8H2O.    Critical  temp,  of  decomposition 
in  open  vessel  =  9.6°;  in  closed  vessel  =  28.7°. 
Solubility  in  H2O. 
%  C12  =  %  of  C12  in  Cl2+Aq  sat.  at  t°  and 
760  mm.  in  presence  of  C12+8H2O. 

t° 

a 

t 

a 

0 
9.2 
9.3 

14.8 

1.6978 
1.2145 
1  .  2068 
0.9740 

15.4 
20.4 
21.9 

0.9511 
0.7758 
0.7385 

t°                 %  CU                  t° 

%CU 

(Kumpf,  W.  Ann.  Beibl.  6.  276.) 

Solubility  of  Cl  in  sat.  NaCl-f-Aq  at  t°  and 
760  mm.  pressure. 

0              0.505            12.5 
3              0.64              20 
6              0.709            28.5 
9              0.900 

1.10 
1.82 
3.50 

(Roozeboom,  R.  t.  c.  1884,  3.  57.) 

Chlorine  wojjoxide,  C12O. 
Sol.  in  H2O.    At  0°,  H2O  absorbs  at  least 
200  times  its  volume  of  C12O  gas. 

Chlorine  dioxide,  C12O3. 
Decomp.  on  air  at  57°  with  explosion. 
H2O  absorbs  5-6  vols.  C1203.     (Millon,  A. 
ch.  (3)  7.  298.) 
H2O  absorbs  at  8.5°  and  753  mm.  press. 
8.591  vols.  C12O3.    (Brandan.) 
100  g.  H2O  dissolve  at: 

f                < 

Coefficient  of  absorp- 
ion  at  0°  and  760  mm. 

Solubility  at  0°  and 
760  mm. 

14.5 
29.0 
60.0 
82.0 

0.3607 
0.3125 
0.1332 

O.G586 

0.3898 

0.3458 
0.1625 
0.0763 

(Kohn  and  O'Brien,  J.  Soc 
17.  1100. 

.  Chem.  Ind.  1898, 

Sat.  KCl+Aq  absorbs  V*  less  Cl  at  15°  than 
pure  H2O.  (Dettmer,  A.  38.  35.) 

1  1.  of  a  solution  of  CaCl2  (1  pt.  in  15  pts. 
H2O)  dissolves  2.45  g.  Cl  at  12°. 

1  1.  of  a  solution  of  MgCl2  (1  pt.  in  15  pts. 
H2O)  dissolves  2.33  g.  Cl  at  12°. 

1  1.  of  a  solution  of  MnCl2  (1  pt.  in  15  pts. 
H2O)  dissolves  2.00  g.  Cl  at  12C. 

SI.  sol.  in  KOH+Aq.    (Fremy.) 

Somewhat  sol.  in  liquid  NO2.  (Frankland, 
Chem.  Soc.  1901,  79.  1361.) 

CC14  absorbs  10%  of  C12  at  13°.  (Perkins, 
Chem.  Soc.  1894,  65.  20.) 

1  mol.  CrOCl2  dissolves  at  0°,  0.70  atom  Cl; 
at- 14°,  1.24  atoms;  at- 21°,  2.31  atoms; 
and  at- 24,  3.00  atoms  Cl.  (Roozeboom,  R. 
t.  c.  4.  379.) 

Sulphuryl  chloiide  absorbs  71  vols.  Cl  or 
0.136  pt.  Cl  by  weight  at  0°.  (Schulze,  J.  pr. 
(2)  27.  168.) 

Insol.  in  benzene.    (Moride.) 

SI.  sol.  in  chloral  and  iodal.    (Dumas.) 

Sol.  in  perchlorethylene.    (Faraday.) 

Sol.  in  a  very  large  quantity  of  ether  with 
decomp. 


8.5°  and  752.9  mm.  press.  4.7655  g.  C12O3. 

14°       "    756.3     "        "     5.0117 

21°       "    754        "        "     5.4447 

93°       "    760        "        "     5.6508 

(Brandan,  A.  161.  340.) 

Does  not  exist,  and  above  data  are  for  mix- 
ture of  C1O2  and  Cl.  (Garzarolli-Thurnlakh, 
A.  209.  184.) 

Chlorine  tefroxide,  C1O2. 

H2O  at  4°  absorbs  about  20  vols.  C1O2  with 
formation  of  HC1O2  and  HC1O3. 

H2SO4  at- 18°  absorbs  about  20  vols.  C1O2. 
(Millon,  A.  ch.  (3)  7.  285.) 

Solubility  of  C1O2  in  H2O. 


t° 

g.  C1O2  per  1. 

1 

10.7 
14.0 

>108.6 
116.7 
>107.9 

ray,  Z.  phys.  Ch.  1906,  54.  569.) 


234 


CHLORINE  OXIDE 


+8H2O  (=fclH2O). 

Lithium  chloriridate,  Li2IrCl6. 

Solubility  in  H2O. 

Somewhat  deliquescent;  very  sol.  in  H2O. 
(Antony,  Gazz.  ch.  it.  23,  1.  190.) 

t° 

g.  C1O2  per  1. 

t° 

g.  C1O2  per  1. 

Potassium  chloriridate,  K2IrCl6. 

0.79* 
0 
1 

26.98 
27.59 

29  48 

10 
15.3 
18  2 

60.06 
60.06 
107  9 

SI.  sol.  in  cold  H2O;  sol.  in  15  pts.  boiling 
H2O;  less  sol.  in  H2O  containing  HC1;  insol. 
in  alcohol  or  sat.  KC1,  and  CaCl2+Aq. 

5.7 

42.10 

Insol.  in  liquid  NH3.      (Gore,  Am.  Ch.  J. 

1898,  20.  829.) 

Entertic. 


(Bray.) 


Chlorine  oxide,  Cl6Oi7. 
Very  easily  decomp.    (Millon,  A.  46.  281.) 
Probably  a  mixture  of  C1O2  and  O. 

Chlorine  Aep/oxide,  C1207. 

Explosive;  decomp.  by  H2O;  sol.  in  well 
cooled  benzene  with  si.  decomp.  (Michael, 
Am.  Ch.  J.  1909,  23.  447.) 

Chlorirididiamine  chloride, 

C1  j  NH3NH3C1. 

ul2lrNH3NH3Cl 

SI.  sol.  in  cold,  easily  in  hot  H2O.  (Skobli- 
koff,  A.  84.  275.) 

nitrate,  Cl2Ir(N2H6NO3)2. 

Sol.  in  H2O. 

-  sulphate,  Cl2Ir(N2H6)SO4. 
SI.  sol.  in  cold,  much  more  easily  in  hot 
H2O. 

Chloriridic  acid. 

Chloriridates. 

Most  of  the  chloriridates  are  very  difficultlv 
sol.  in  H2O,  but  a  little  more  sol.  than  the 
corresponding  chloroplatinates.  Insol.  or 
nearly  so  in  alcohol,  but  not  so  difficultly  sol. 
as  the  chloroplatinates.  (Rose.) 

Ammonium  chloriridate,  (NH4)2IrCl6. 

Sol.  in  20  pts.  cold  H2O  (Vauquelin);  si. 
sol.  in  cold,  much  more  in  hot  H2O  (Glaus) ; 
sol.  in  HCl+Aq  (Soblewsky);  insol.  in  cold 
NH4Cl+Aq  (Glaus);  insol.  in  alcohol  (Ber- 
zelius). 

100  pts.  H2O  dissolve  at: 
14.4°     26.8°     39.4° 
0.699    0.905     1.226  pts.  (NH4)2IrCl6, 
52.2°     61.2°     69.3° 
1.608    2.130    2.824  pts.  (NH4)2IrClc. 
(Rimbach  and  Korten,  Z.  anorg.  1907,  52. 
407.) 

Caesium  chloriridate,  Cs2IrCl6. 

Only  si.  sol.  in  H^O.  (Delepine,  C.  R.  1908, 
146.  1268.) 


Rubidium  chloriridate,  Rb2lrCl6. 

Very  si.  sol.  in  H2O.  (Rimbach,  Z.  anorg. 
1907,  52.  408.) 

Sodium  chloriridate,  Na2IrClG+6H2O. 

Easily  sol.  in  H2O;  sol.  in  alcohol  of  0.837 
sp.  gr. 

Thallium  chloriridate,  Tl2IrCl6. 

Decomp.  by  hot  HC1  forming  Tl3IrCl6. 
(Delepine,  C.  R.  1909,  149.  1073.) 

Chloriridium  pentamine  comps. 
See  Iridope^amine  chloro  comps. 

Chloriridosulphuious  acid. 

Potassium  chloriridosulphite.  K4Ir2Cl2(SO3)4, 
4KC1+12H2C 

Insol.  in  cold,  decomp.  by  hot  H2O. 

K4lr2Cl2(S03)4,  2K2SO3.    Decomp.  by  H2O. 

Cl2Ir2(S03)2,  8KC1+4H2O.  Sol.  in  H2O; 
insol.  in  alcohol.  (Glaus,  J.  pr.  42.  354.) 

Chloriridous  acid. 

Ammonium  chloriridite,  (NH4)3IrCl6. 

Decomp.  by  H2O.    (Delepine,  C.  R.  1908, 

146.  1268.) 

+  1KH2O.    Sol.  inH2O.    (Glaus.) 
IrCl5(H2O)  (NH4)2.    (Delepine.) 

Caesium  chloriridite,  IrCl5(H2O)Cs2. 
(Delepine.) 

Lithium  chloriridite,  Li3IrCl6+12H2O. 

Deliquescent;  sol.  in  H2O  and  alcohol. 
(Delepine,  C.  R.  1914,  158.  1277.) 

Lithium  sodium  chloriridite,  Li2NaIrCl6  + 
12H2O. 

Stable  in  aq.  solution  in  the  presence  of 
excess  of  lithium  salt.  (Delepine,  C.  R.  1914, 
158.  1278.) 

LiNa2IrCl6+12H2O.  Stable  in  aq.  solu- 
tion in  the  presence  of  excess  of  sodium  salt. 
(Delepine,  C.  R.  1914,  158.  1278.) 

Potassium  chloriridite,  K3IrCl6. 

Decomp.  by  H20.    (Delepine.) 

+3H2O.  Easily  sol.  in  H2O;  insol.  in  al- 
cohol; insol.  in  sat.  KCl+Aq.  (Berzelius.) 

IrCl5(H2O)K2.    (Delepine.) 


CHLOROCOLUMBIUM  CHLORIDE 


235 


Rubidium  chloriridite,  IrCl5(H2O)Rb2. 
(Delepine.) 

Silver  chloriridite,  Ag3IrCl6. 

Insol.  in  H20  or  acids;  si.  sol.  in  NH4OH  + 
Aq. 

Ppt.    (Delepine,  Bull.  Soc.  1910,  (4),  7.  55.) 

Sodium  chloriridite,  Na3IrCl6  +  12H2O. 

Efflorescent;  sol.  in  ^  pt.  H20.    Insol.  in 
alcohol.    Melts  in  crystal  H2O  at  50°. 

Thallium  chloriridite,  Tl3IrCl6. 

Sol.  in  hot  HC1;  pptd.  on  cooling.    (Dele- 
pine,  C.  R.  1909,  149.  1073.) 

Chlorofeframine  chromium  comps. 
See  Chlorotetramine  chromium  comps. 

Chloro-azoimide,  N3C1. 

SI.  sol.  in  H20.     (Raschig,  B.   1908,  41. 
4194.) 

Chlorobromo  comps: 
See  Bromochloro  comps. 

Chlorocarbonic  acid. 
See  Carbonyl  chloride. 


Chlorochromic  acid. 


Known  only  in  its  salts. 
CrO2Cl2.    See  Chromyl  chloride. 

Ammonium    chlorochromate,    NH4CrO3Cl  = 

Cr°2ONH4. 

More  sol.  in  H2O  than  the  K  salt.  (Peligot, 
A.  ch.  52.  283.) 

Barium  chlorochromate  chloride, 
Ba(Cr03Cl)2,  BaCl2. 

Deliquescent.  Very  sol.  in  H2O.  (Prator- 
ius,  A.  201.  1.) 

+H2O.    Not  deliquescent. 

Calcium  chlorochromate,  Ca(OrO3Cl)2. 

Deliquescent.    (Peligot.) 

+5H2O.    Very  deliquescent.     (Pratorius.) 

Chromous  chlorochromate. 
See  Tn'chromyl  chloride. 

Cobalt  chlorochromate,  Co(CrO3Cl)2+9H2O. 
Deliquescent;  melts  at  40°  in  crystal  H2O. 

(Pratorius.) 

Lithium  chlorochromate,  LiCrO3Cl. 

Sol.  in  H2O  acidified  with  HC1  without 
decomp.  (Lowenthal,  Z.  anorg.  1894,  6. 
357.) 


Magnesium  chlorochromate,  Mg(CrO3Cl)2. 

Deliquescent.    (Peligot.) 

-f  9H2O.  Less  deliquescent  than  the  other 
chlorochromates.  (Pratorius,  A.  201.  1.) 

Very  hydroscopic;  sol.  in  H2O  acidified 
with  HC1  without  decomp.  (Lowenthal,  Z. 
anorg.  1894,  6.  359.) 

Nickel  chlorochromate,  Ni(CrO3Cl)2-f9H2O. 
Deliquescent;  melts  in  its  crystal  H2O  at 
4&-480.    (Pratorius.) 

Potassium  chlorochromate,  KCrO3Cl  = 
CrO2(Cl)OK. 

Sol.  in  H2O  with  decomp.  Cryst.  from  H2O 
containing  HC1  without  decomp.  (Peligot.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

Sodium  chlorochromate,  NaCrO3Cl. 
Deliquescent.    (Peligot.) 
+2H2O.    Deliquescent.    (Pratorius.) 

Strontium  chlorochromate,  Sr(CrO3Cl)2  + 
4H2O. 

Deliquescent;  melts  in  crystal  H2O  at  72°. 
(Pratorius.)  • 

Thallous  chlorochromate,  TlCrO3Cl. 

Decomp.  by  H20.  (Lachaud  and  Lepierre, 
C.  R.  103.  198.) 

Zinc  chlorochromate,  Zn(CrO3Cl)2+9H2O. 

Deliquescent;  melts  at  37.5°  in  crystal  H2O. 
(Pratorius.) 

Very  hydroscopic;  very  sol.  in  H2O  and 
acids.  (Lowenthal,  Z.  anorg.  1894,  6.  360.) 

ZHchloro  chromium  bromide, 

[Cr(H2O)4Cl2]Br. 

Very  deliquescent.  Sol.  in  fuming  HBr, 
in  a  mixture  of  equal  volumes  ether  and  fum- 
ing HBr,  in  alcohol  and  in  acetone.  (Bjerrum, 
B.  1907,  40.  2919.) 

Chlorochromotetrammonium  comps. 
See  Chlcrotetramine  chromium  comps. 

Chlorocolumbium  bromide,  (Cb8Cli2)Br2-h 

7H20. 

Sol.  in  a  small  quantity  of  cold  H2O. 
(Harned,  J.  Am.  Chem.  Soc.  1913,  36.  1083.) 

Chlorocolumbium  chloride,  (Cb6Cli2)Cl2  + 
7H2O. 

Insol.  in  cold,  sol.  in  boiling  H2O. 

Not  easily  decomp.  by  boiling  with  NH4OH. 
Cone.  HN03  decomp.  a  boiling  solution  of 
this  comp.  Completely  sol.  in  cone,  alkalies. 
(Harned,  J.  Am.  Chem.  Soc.  1913,  36.  1080.) 


236 


CHLOROCOLUMBIUM  HYDROXIDE 


Chlorocolumbium  hydroxide,  (Cb6Cli2)  (OH)2 

+8H2O. 

Insol.  in  H2O.    Sol.  in  acids  and  alkalies. 
(Earned,  J.  Am.  Chem.  Soc.  1913,  35.  1082.) 

Chloroctamine  cobaltic  carbonate, 
Cl4Co2(NH3)8CO3+2H2O. 

Very  sol.  in  H2O.     (Vortmann  and  Bias- 
berg,  B.  22.  2651.) 

Cl2Co2(NH3)8(CO3)2+H2O.      (Vortmann 
and  Blasberg.) 

Chloroferrous  acid. 
Calcium  chloroferrite,  CaO,  CaCl2,  Fe2O3. 
Insol.  in  H2O.    (le  Chatelier,  C.  R.  99.  276.) 

Di'chlorofulminoplatinum, 

Pt4N4Cl2012H22(?). 
Insol.  in  H2O.     (v.  Meyer,  J.  pr.  (2)  18. 

305.) 

Y'n'chlorofulininoplatinum, 

Pt4N4Cl3(OH)012H24(?). 
Insol.    in    H2O;    sol.    in    HCl+Aq.      (v. 
Meyer.) 

T^racUorofulminoplatinum, 

Pt4N4Cl4012H24(?) 
Insol.  in  H2O.    (v.  Meyer.) 

Chlorohydroxylonitritoplatin6e?m'di- 
amine  nitrite,  (OH)ClNO2Pt(NH3)2NO2. 
Easily  sol.  in  hot  H20.    (Cleve.) 

Chlorohydroxyloplatindi'amine  bromide, 


SI.  sol.  in  H2O. 

-  carbonate, 

Insol.  in  H2O.    (Cleve.) 

-  chloride,  O 

81.  sol.  in  HjO.    (Cleve.) 


Nearly  insol.  in  H20. 


Ppt.    (Cleve.) 

—  •  nitrate  (Raewsky's  nitrate), 


SI.  sol.  in  cold,  more  easily  in  hot  H2O. 
(Gerhardt.) 

Chlorohyposulphuric  acid,  S2O3C14. 
fee  Sulphur  oxy^rachloride. 


Chloromanganic  acid. 
Se3  Manganic  hydrogen  chloride. 

Chloromercurosulphrous  acid. 

Ammonium  chloromercurosulphite, 

NH4SO3HgCl. 
Sol.  in  H2O.    (Earth,  Z.  phys.  Ch.  9.  205.) 

Barium  chloromercurosulphite, 

Ba(SO3HgCl)2. 
Insol.  in  H2O.    (Barth.) 

Potassium  chloromercurosulphite,  KSO8HgCl. 
Sol.inH20.    (Barth.) 

Sodium  chloromercurosulphite,  NaSO3HgCl 

+H20. 
Very  sol.  in  H20.    (Barth.) 

Chloromolybdenum  bromide, 
Cl4Mo3Br2+3H2O. 

Insol.  in  H2O  and  dil.  acids;  sol.  in  alcohol. 

+6H2O.  At  first  easily  sol.  in  H2O,  but  a 
precipitate  soon  forms.  Can  be  crystallized 
from  dil.  HBr+Aq.  Sol.  in  alcohol  and  ether. 
(Blomstrand.) 


bromide, 


Chloromolybdenum  potassium 
Cl4Mo3Br2,  2KBr+2H2O. 
Decomp.  by  H2O.    Can  be  cryst.  from  HBr 
-fAq.    (Blomstrand.) 

Chloromolybdenum  chloride,  Cl4Mo3Cl2  = 
molybdenum  ^'chloride,  MoCl2. 

Insol.  in  H2O;  easily  sol.  in  HCl+Aq  or 
H2SO4+Aq;  si.  sol.  in  HN03;  sol.  in  NH4OH 
+Aq,  NaOH+Aq,  or  KOH-fAq,  with  sep- 
aration of  precipitate  on  boiling;  sol.  in 
alcohol  and  ether.  (Blomstrand,  J.  pr.  77. 
96.) 

Very  sol.  in  cone.  HC1.  (Rosenheim  and 
Kohn,  Z.  anorg.  1910,  66.  2.) 

+3H2O.    Insol.  in  H2O. 

+4i£H2O.  Insol.  in  H2O.  (Liechti  and 
Kempe,  A.  170.  351.) 

+6H2O.  Sol.  in  H20,  alcohol,  or  ether. 
(Blomstrand.) 

Chloromolybdenum  hydrogen  chloride, 

Mo3Cl6,  HC1+4H20. 

Sol.  in  H2O,  but  ppt.  forms  after  a  few 
minutes.  (Rosenheim  and  Kohn,  Z.  anorg. 
1910,  66.  5.) 

Chloromolybdenum  potassium  chloride, 

Cl4Mo3Cl2,  2KC1+2H2O. 
Decomp.  by  pure  H2O;  can  be  recrystal- 
lized  from  HCl+Aq.    (Blomstrand,  J.  pr.  77. 
108.) 


CHLORONITRITE,  IRIDIUM  POTASSIUM 


237 


Chloromolybdenum  hydroxide,  Cl4Mo3(OH2) 
+2H20. 

Insol.  in  H2O  or  alcohol.  Easily  sol.  in 
strong  acids  if  fresh,  and  washed  only  with 
cold  H2O.  If  washed  with  warm  H20,  it  is 
less  sol.  in  acids.  If  precipitated  hot,  is  insol. 
in  acids,  even  H2SO4  or  fuming  HNO3.  (Blom- 
strand,  J.  pr.  77.  100.) 

+8H2O. 

Chloromolybdenum  iodide,  Cl4Mo3I2+3H2O. 
Precipitate. 
+6H2O.    Sol.  in  H2O  and  alcohol. 

Chloromolybdenum  potassium  iodide, 

Cl4Mo3I2,  2KI+2H2O. 
Decomp.  by  H2O.    Recryst.  from  HI+Aq. 
(Blomstrand.) 

OTT 

Chloromolybdenum  oxybromide,  Cl4Mo3  gr 

+2H2O. 

Insol.  in  alcohol.  (Blomstrand,  J.  pr.  77. 
116.) 

Chlcromolybdic  acid, 

MoOCl3(OH)+7H2O. 
Very  hydroscopic.    (Weinland,  B.  1904,  37. 

572.) 

Di'ammonium  tefrachloromolybdate, 

MoCl4(ONH4)2+2H20. 
Hydroscopic.     Decomp.  by  H2O.     Sol.  in 
dilute  acids,  alkalies  and  ammonia.    (Wein- 
land, Z.  anorg.  1905,  44.  83.) 

Caesium  chloro/ranolybdate,  acid, 

Mo6OuCl14(Cs20)+22H20. 
Hydroscopic.     Decomp.  by  H2O.     Sol.  in 
dilute  acids,  alkalies,  and  ammonia.    (Wein- 
land, I.e.} 

Monoc&siwa.  Jn'chloromolybdate, 

MoOCl3(OCs)+H20. 

Hydroscopic.  Decomp.  by  H2O.  Sol.  in 
dilute  acids,  alkalies  and  ammonia.  (Wein- 
land.) 

ZH'csesium  fc^rachloromolybdate, 

MoCl4(OCs)2. 

Hydroscopic.  Sol.  in  H2O  with  decomp. 
Sol.  in  dilute  acids,  alkalies,  and  ammonia. 
(Weinland,  Z.  anorg.  1905,  44.  83.) 

Morcopotassium  Zn'chloromolybdate, 

MoOCl3(OK)+H2O. 

Hydroscopic.  Decomp.  by  H2O.  Sol.  in 
dilute  acids,  alkalies,  and  ammonia.  (Wein- 
land.) 

Dipotassium  tefrachloromolybdate, 

IVLC14(OK)2+2H2O. 

Hydroscopic.  Decomp.  by  H2O.  Sol.  in 
dilute  acids,  alkalies,  and  ammonia.  (Wein- 
land.) 


Potassium  hydrogen  jchloro/rimolybdate, 

Mo60uri14,  K2O+6H2O. 
Hydroscopic.     Decomp.  by  H2O.     Sol.  in 
dilute  acids,  alkalies,  and  ammonia.    (Wein- 
land.) 

Afoworubidium  fnchloromolybdate, 

MoOCl3(ORb)+H20. 
Hydroscopic.     Decomp.  by  H2O.     Sol.  in 
dilute  acids,  alkalies,  .and  ammonia.    (Wein- 
land.) 

Dirubidium  tefrachloromolybdate, 

MoCl4(ORb)2. 

Hydroscopic.  Decomp.  by  H20.  Sol.  in 
dilute  acid,  alkalies,  and  ammonia.  (Wein- 
land.) 

Chloronitratoplatinamine  nitrite, 


Easily  sol.  in  H2O. 
Chloronitratoplatindx'amine  nitrate, 


Decomp.    by    H2O    with    formation    of 
0^Pt[(NH3)2N03)]2. 


-  sulphate,  iC^Pt(N2H6)2S04+H20. 
SI.  sol.  in  cold,  more  easily  in  hot  H2O. 

Chloronitritotetramine  cobaltic  chloride, 

Cl(N02)Co(NH3)4Cl. 

Not  very  sol.  in  cold  H20.    (Jorgensen,  Z. 
anorg.  5.  195.) 


Chloromtritoplatinse/mdmmine  chloride, 

Cl2(N02)Pt(NH3)2Cl. 
100  pts.  solution  in  H20  sat.  at  18°  contain 
1.8  pts.  salt;  sat.  at  100°,  6  pts. 

Insol.  in  abs.  alcohol  or  ether.  Not  decomp. 
by  cone.  HNO3,  HC1,  or  H2C2O4+Aq,  and  by 
H2SO4  only  at  a  high  heat. 

Formula  given  was  PtNeHiaCleO*.     (Pey- 
,  J.  B.  1865.  421.) 


rone, 


nitrite,  Cl2(N02)Pt(NH3)2N02. 

Sol.  in  H2O.    (Blomstrand.) 

Chlorophosphatoplatincfaamine    phos- 

ClPt(N2H6)2 
phate,       \    /     +2H2O. 

PO4 

Nearly  insol.  in  cold,  and  only  very  si.  sol. 
inhotH2O.    (Raewsky.) 

Chloronitrous  acid. 

Indium  potassium  chloronitrite,  Ir2Cl2(NO2)4, 

6KC1, 

Ppt.;  decomp.  by  boiling  H2O.    Sol.  in  cold 
H2O.    (Leidi^,  C.  R.  1902,  134.  1583.) 


238 


CHLOROPALLADIC  ACID 


Ir3KJ2Cl16(NO2)8+4H20.  Ppt.  (Quen- 
nessen,  C.  R.  1905,  141.  258.) 

Chloropalladic  acid. 
Chloropalladates. 

The  chloropalladates  are  generally  very  sol. 
in  H2O,  and  sol.  in  alcohol,  (v.  Bonsdorff, 
Pogg.  17.  264.) 

Ammonium  chloropalladate,  (NH4)2PdCl6. 
SI.  sol.  in  H20.    (Berzelius.) 

Barium  chloropalladate. 

Sol.  in  H2O  and  alcohol,    (v.  Bonsdorff.) 

Cadmium  chloropalladate. 
As  above. 

Caesium  chloropalladate,  Cs2PdCl6. 

Nearly  insol.  in  cold  H2O.  Decomp.  by 
boiling  with  H2O  or  by  hot  cone.  H2SO4. 
(Gutbier,  B.  1905,  38.  2386.) 

Calcium  chloropalladate. 

Deliquescent;  sol.  in  H2O  and  alcohol,  (v. 
Bonsdorff,  1829.) 

Glucinum  chloropalladate,  GlPdCl6-f8H2O. 
Very  hydroscopic,  and  sol.  in  H2O. 

Magnesium  chloropalladate,  MgPdCl6+ 
6H2O. 

Deliquescent;  sol.  in  H2O. 

Nickel  chloropalladate,  NiPdCl6+6H2O. 
Extremely  deliquescent. 

Potassium  chloropalladate,  K2PdCl6. 

SI.  sol.  in  cold  H2O.  Decomp.  by  long  boil- 
ing with  H2O.  SI.  sol.  in  dil.  HCl+Aq  with- 
out decomp.  Insol.  in  NH4C1,  KC1,  or  NaCl 
H-Aq.  Insol.  in  alcohol.  (Berzelius.) 

Rubidium  chloropalladate,  Rb2PdCl6. 

Insol.  in  cold  H2O.  Decomp.  by  boiling 
with  H2O  or  by  hot  cone.  H2SO4.  (Gutbier, 
B.  1905,  38.  2387.) 

Zinc  chloropalladate,  ZnPdCl6+6H2O. 
Very  deliquescent,    (v.  Bonsdorff.) 

Chloropalladous  acid 

Aluminum  chloropalladite,  Al2Pd2Cli0+ 
20H2O. 

Deliquescent.  Sol.  in  H2O,  alcohol,  or 
ether.  (Welkow,  B.  7.  804.) 

Ammonium   chloropalladite,    (NH4)2PdCl4+ 

H2O. 

Easily  sol.  in  H2O.  Insol.  in  alcohol.  Sol 
inNH4Cl+Aq.  (Glaus.) 


Easily  sol.  in  H2O.    (Gutbier,  B.  1905,  38. 
2386.) 

Barium  chloropalladite. 

Easily  sol.  in  H2O  or  alcohol. 

Cadmium  chloropalladite. 
Not  deliquescent. 

Caesium  chloropalladite,  Cs2PdCl4. 

Can  be  cryst.  from  hot  H2O.    (Gutbier,  B: 
1905,  38.  2386.) 

Calcium  chloropalladite. 
Deliquescent.    Sol.  in  H2O  or  alcohol. 


Glucinum  chloropalladite,  GlPdCl4+6H2O. 

Very  hygroscopic; 
or  ether.    (Welkow.) 


Very  hygroscopic;  very  sol.  in  H2O,  alcohol, 
.    (We 


Magnesium  chloropalladite. 

Deliquescent.  Easily  sol.  in  H2O.  (v. 
Bonsdorff.) 

Manganese  chloropalladite. 
Sol.  in  H20  and  alcohol. 

Nickel  chloropalladite. 
Sol.  in  H2O. 

Potassium  chloropalladite,  K2PdCL. 

Much  more  sol.  in  hot  than  cold  H2O. 
(Joannis,  C.  R.  96.  295.)  Sol.  in  NH4OH+ 
Aq.  (Berzelius.)  Sol.  in  cold  sat.  KCl+Aq. 
(Gibbs,  Sill.  Am.  J.  (2)  31.  70.)  Insol.  in  al- 
cohol. (Wollaston.)  Somewhat  sol.  in  al- 
cohol of  0.84  sp.  gr.,  but  insol.  in  absolute  al- 
cohol; decomp.  on  boiling  (Berzelius.) 

Rubidium  chloropalladite,  Rb2PdCl4. 

Can  be  cryst.  from  hot  H2O.  (Gutbier,  B. 
1905,  38.  2387.) 

Sodium  chloropalladite. 

Deliquescent.    Sol.  in  H2O  and  alcohol. 

Zinc  chloropalladite. 

Very  deliquescent.  Sol.  in  H2O  and  alcohol. 
(v.  Bonsdorff.) 

Chlorophosphoarsenioiridic  acid,  2IrCl3. 

3H3P03,  3H3P04,  5H3As04(?). 
Very  sol.  in  H20.    (GeisenheimerJ 

Lead  chlorophosphoarsenioiridate,  4IrCl3, 
3Pb2H2(P03)2,  3Pb,(P04)*, 

5Pb2H2(AsO4)2. 
Insol.  in  H2O. 

Chlorophosphoiridic  acid,  2IrCl3,  3H3PO4, 
3H3PO3. 

Very  sol.  in  H2O.  Insol.  in  alcohol. 
(Geisenheimer,  A.  ch.  (6)  23.  254.) 

2IrCl3j  3H3PO4.    Sol.  in  H2O  and  alcohol. 


CHLOROPLATINATE,  AMMONIUM 


239 


Ammonium     chlorophosphoiridate,     2IrCl3, 

3(NH4)3P04,  3(NH4)2HP03. 
Very    deliquescent.      Very    sol.    in    H20. 
(Geisenheimer.) 

Lead  chlorophosphoiridate,  4IrCl3, 

3Pb3(P04)2,  3PbH2(P03)2. 
Insol.  in  H2O  or  acetic  acid;  very  sol.  in  dil. 
HNOs+Aq.    (Geisenheimer.) 

Silver  chlorophosphoiridate,  2IrCl3, 

3AgH2PO4,  3AgH2PO3. 
Insol.  in  H2O.     Sol.  in  HNO3+Aq,  and 
NH4OH+Aq.    (Geisenheimer.) 

Chlorophosphoplatinic  acid. 
See  Chloroplatinophosphoric  acid. 

Chlorophosphoric  acid. 

Thorium  chlorophosphate,  3ThO2,ThCl4, 

2P206. 

Insol.  in  H2O  and  acids;  decomp.  by  boil- 
ing with  H2SO4  and  fusing  with  alkali  car- 
bonates. (Golani,  C.  R.  1909,  149.  208.) 

Chloroplatinamine  chloride,  C^Pt^^j1 

Sol.  in  about  700  pts.  H2O  at  0°,  and  33-34 
pts.  at  100°.  Not  attacked  by  boiling  cone. 
HNO3  or  H2SO4.  Sol.  in  boiling  KOH+Aq 
with  decomp.  Sol.  in  NH4OH+Aq.  (Cleve, 
Sv.  V.  A.  H.  10,  9.  30.) 

—  nitrite,  Cl2Pt(NH3NO2)2. 


SI.  sol.  in  cold,  easily  in  hot  H2O. 

nitrite  silver  nitrite,  Cl2Pt(NH3N02)2, 


AgN02. 

Easily  sol.  in  hot,  si.  sol.  in  cold  H2O. 
(Cleve.) 


nitritochloride, 


Sol.  in  H2O.    (Cleve.) 

CMoroplatinefa'amine  bromide, 

Cl2Pt(N2H6Br)2. 
SI.  sol.  in  hot  H2O.    (Cleve.) 

-  chloride  (Gros'.  chloride), 
Cl2Pt(N2H6Cl)2. 

Nearly  insol.  in  cold,  and  only  si.  sol.  in  hot 
H2O.  Sol.  in  hot  cone.  KOH+Aq,  with  de- 
comp. (Grimm.) 

Sol.  in  cold  KOH+Aq  without  decomp. 
Nearly  insol.  in  NH4OH+Aq.  (Buckton.) 


+ 


y  n 
H2O. 


(Raewsky.) 


—  chloroplatinate,  NCl2Pt(2H6Cl)2,  PtCl4. 
Easily  sol.  in  hot  H2O. 

—  -  chloroplatinite,  Cl2Pt(N2H6Cl)2,  PtCl2. 
SI.  sol.  in  H20.    (Cleve.)    . 


Chloroplatintfiamine  chromate, 

Cl2Pt(N2H6)2CrO4. 
Nearly  insol.  in  H2O.    (Cleve.) 

—bichromate,  Cl2PtfN2H6)2Cr2O7. 
SI.   sol.  in  cold,   more  sol.   in  hot  H2O. 
(Cleve.) 

-  nitrate  (Gros'  nitrate),Cl2Pt(N2H6NO8)2. 
Much  more  easily  sol.  in  hot  than  in  cold 
H2O.     Sol.  in  hot  KOH+Aq  with  decomp. 
Nearly  insol.  in  cone.  HNO3+Aq. 


-  nitritochloride, 
Ppt.    (Jorgensen.) 

-  phosphate. 

See  Chlorophosphatoplatin^'amine  phos- 
phate. 

-  sulphate,  Cl2Pt(N2H6)2SO4. 

SI.  sol.  in  both  cold  or  hot  H2O.    (Cleve.) 
+rcH2Q.     SI.  sol.  in  cold,  easily  in  hot 
H2O.    (Grimm.) 

--  sulphocyanide,  Cl2Pt(N;>H6)2(CNS)2 

+H20. 
Ppt.    (Cleve.) 

Chloroplatinwonodi'amine  chloride, 

ri  p,  (NH3)2C1 
Cl2PfcNH3Cl. 
Quite  easily  sol.  in  H2O.    (Cleve.) 

Chloroplatinsewidz'amine  carbonate  chlo- 

ride, 2Pt(NH3)2Cl2,  Pt2(NH3)4Cl2(C03). 

SI.  sol.  in  H2O;  insol.  in  alcohol  and  ether. 

Decomp.  by  cold  HC1  +Aq  .    (Schon,  Z.  anorg. 

1897,  13.  37.) 

Chloroplatinsewiefo'amine  chloride, 

Cl3Pt(NH3)2Cl. 

Sol.  in  300  pts.  H2O  at  0°,  and  65  pts.  at 
100°.  Not  decomp.  by  cone.  H2SO4.  Sol.  in 
KOH+Aq  without  decomp.  (Cleve.) 

Chloroplatinic  acid,  H2PtCl6+6H2O. 

Dehquescent.  Sol.  in  H20,  alcohol,  or  ether. 
+4H2O.     Deliquescent.     (Pigeon,   C.  R. 
112.  1218.) 
PtCl4,  HC1+2H2O.    (Pigeon.) 

Aluminum  chloroplatinate,  A1C13,  PtCl4+ 
15H2O. 

Very  sol.  in  H2O  and  alcohol.  (Welkow,  B. 
7.  304.) 

Insol.  in  ether. 

Ammonium  chloroplatinate,  (NH4)2PtCl6. 

SI.  sol.  in  cold,  more  easily  in  hot  H2O. 
(Fresenius.) 

100  ptSi  H2O  dissolve  0.666  pt.  at  ord. 
temp,  and  12.5  pts.  at  100°.  (Crookes,  C.  N. 
9.37.)  . 


240 


CHLOROPLATINATE,  BARIUM 


Insol.  in  cold  HCl+Aq.  Separates  out  on 
cooling  from  solution  in  hot  HC1,  HNO3,  or 
H2S04.  (Fischer.) 

Very  si.  sol.  in  cold,  easily  in  hot  NH4OH  + 
Aq.  (Fresenius.) 

Cone.  NH4Cl+Aq  ppts.  it  almost  com- 
pletely from  aqueous  solution.  (Bottger-.) 

Sol.  in  NH4  succinate+Aq.    (Dopping.) 

Less  sol.  in  H2PtCl6+Aq  than  in  H2O. 
(Rogojski,  A.  ch.  (3)  41.  452.) 

Sol.  in  SnCl2+Aq.    (Fischer.) 

Very  sol.  with  decomp.  in  KCNS+Aq. 
(Glaus.) 

At  15-20°,  sol.  in  26,535  pts.  97.5%  alcohol, 
in  1476  pts.  76%  alcohol,  and  in  665  pts.  55% 
alcohol.  If  free  HC1  is  present,  it  is  sol.  in 
672  pts.  76%  alcohol.  (Fresenius,  A.  69.  118.) 

Insol.  in  absolute  alcohol  or  ether. 

Barium  chloroplatinate,  BaPtCl6+6H2O. 

Permanent;  sol.  in  H2O;  decomp.  by 
alcohol,  (v.  Bonsdorff,  Pogg.  17.  250.) 

Barium  rwonochloroplatinate,  PtCl(OH)5Ba+ 

H20. 

Insol.  in  H2O  and  in  org.  solvents.  (Bel- 
lucci,  C.  C.  1903,  1.  131.) 

Barium  pe/itachloroplatinate,  OH.PtCl5Ba-f- 
H20. 

(Miolati,  Chem.  Soc.  1900,  78.  (2)  732.) 
Cadmium  chloroplatinate,  CdPtCl6+6H2O. 

Deliquescent,  and  easily  sol.  in  H2O.  (v. 
Bonsdorff.) 

Caesium  chloroplatinate,  Cs2PtCl6. 
100  pts.  H20  dissolve  at: 
0°  10°          20°          30° 

0.024      0.050      0.079      0.110  pts.  Cs2PtCl6, 
40C  50°          60°          70° 

0.142      0.177      0.213      0.251  pts.  Cs2PtCl6, 
80°          90°        100° 

0.291      0.332      0.377  pts.  Cs2PtCl6. 

(Bunsen,  Pogg.  113.  337.) 

Sol.  in  1308  pts.  H2O  at  15°,  and  261  pts.  at 
100°.  (Crookes,  C.  N.  9.  205.) 

Calcium  chloroplatinate,  CaPtCl6+8H2O. 

Deliquescent;  easily  sol.  in  H2O.  (v.  Bons- 
dorff.) 

Calcium   wonochloroplatinate,  PtCl(OH)6Ca 

+H20. 

Insol.  in  H2O  and  in  org.  solvents.  (Bel- 
lucci,  C.  C.  1903,  I.  131.) 

Cerium  chloroplatinate,  CeCl3,  PtCl4+13H2O. 

Deliquescent;  very  sol.  in  H2O  or  alcohol; 
insol.  in  ether.  (Marignac.) 

4CeCls,  3PtCl4+8H2O.  Deliquescent; 
easily  sol.  in  H2O  or  alcohol;  insol.  in  ether. 
(Holzmann,  J.  pr.  84.  80.) 

Chromium   chloroplatinate,    CrCl3,    PtCl4+ 


Deliquescent.    (Nilson,  B.  9.  1056.) 


+10H2O.  Very  sol.  in  H2O  and  alcohoL 
Nearly  insol.  in  acetone.  (Higley,  J.  Am. 
Chem.  Soc.  1904,  26.617.) 

Cobalt  chloroplatinate,  CoPtCl6+6H20. 

Very  deliquescent.    (Jorgensen.) 
Copper  chloroplatinate,  CuPtCl6+6H2O. 

Deliquescent  in  moist  air.    (v.  Bonsdorff.} 

Didymium  chloroplatinate,  DiCl3,  PtCl4+ 
13H2O. 

Less  deliquescent  than  the  cerium  salt. 
(Marignac.) 

+10^H20.  Deliquescent.  (Cleve,  Bull. 
Soc.  (2)  43.  361.) 

Erbium   chloroplatinate,   ErCl3,    PtCl4+ 

11H2O. 
Very  deliquescent.    (Cleve.) 

Gadolinium  chloroplatinate,  GdCl3,  PtCl4+ 
10H20. 

Ppt.  (Benedicko,  Z.  anorg.  1900,  22.  204.) 
Glucinum  chloroplatinate,  GlPtCl6+8H20. 

Deliquescent  in  moist  air.  Very  sol.  in 
H2O,  moderately  in  alcohol.  Insol.  in  ether. 
(Welkow,  B.  6.  1288.) 

Indium    chloroplatinate,    2InCl3,    5PtCl4  + 

36H2O. 
Deliquescent.    (Nilson.) 

Iron     (ferrous)     chloroplatinate,    FePtCl6+ 

6H2O. 

Deliquescent.    (Topsoe.) 
Iron  (ferric)  chloroplatinate,  FeCl3,  PtCl4-f 


Deliquescent.    (Nilson.) 

Lanthanum  chloroplatinate,  LaCls,  PtCl4+ 

13H2O. 

Deliquescent;  extremely  sol.  in  H2O. 
(Cleve.) 

Lead  chloroplatinate,  PbPtCl6+3H2O. 

Easily  sol.  in  H2O  and  alcohol  (Topsoe), 
with  decomp.  (Birnbaum,  Zeit.  Oh.  1867. 
520.) 

Lead     wo/iochloroplatinate,    [PtCl(OH)6]Pb, 

Pb(OH)2. 

Ppt.  (Bellucci,  Chem.  Soc.  1902,  82,  II. 
155.) 

Lead  pentachloroplatinate,  basic, 

PtCl6(OH)Pb,  Pb(OH)2. 
(Miolati,  Chem.  Soc.  1900,  78.  (2)  732.) 

Lithium  chloroplatinate,  Li2PtCl6-|-6H2O. 

Extremely  deliquescent  (Jorgensen)  ;  efflor- 
escent. Easily  sol.  in  H2O,  alcohol,  or  ether- 
alcohol;  insol.  in  ether.  (Scheibler.) 

Lithium  perctachloroplatinate,  OH.PtCl6Li2. 
Very   hydroscopic.      (Miolati,   Chem.   Soc. 
1900,  78  (2)  732.) 


CHLOROPLATINAXE,  POTASSIUM 


241 


Magnesium  chloroplatinate,  MgPtCl6+6H2O. 
Sol.  in  H2O  and  abs.  alcohol. 
+12H2O.    Sol.  in  H2O. 

Manganese  chloroplatinate,  MnPtCl6+6H2O. 
Not  deliquescent;  sol.  in  H2O. 
+12H2O.    SI.  efflorescent. 

Nickel  chloroplatinate,  NiPtCl6+6H2O. 
Sol.  in  H20. 

Potassium  chloroplatinate,  K2PtCl6. 

100  pts.  H20  dissolve  at: 
0°      10°    20°    30°     40°    50° 
0.74  0.90  1.12   1.41   1.76  2.17  pts.  K2PtCl6, 
60°       70°       80°       90°      100° 
2.64     3.19     3.79     4.45     5.18  pts.  K2PtCl6. 
(Bunsen,  Pogg.  113.  337.) 


Sol.  in  KOH+Aq.  Insol.  in  cold  or  hot 
alkali  carbonates  or  bicarbonates+Aq.  (Rose. 

Easily  sol.  in  warm  Na2S2O3 + Aq.   (Himly.) 

Sol.  in  NH4Cl+Aq.    (Brett.) 

Sol.  in  NH4  succinate+Aq.    (Dopping.) 

At  15-20°,  sol.  in  12,083  pts.  absolute  al- 
cohol, in  3775  pts.  76%  absolute  alcohol,  and 
in  1053  pts.  55%  absolute  alcohol.  (Fresen- 
ius.) 

Sol.  in  1835  pts.  76%  alcohol  containing 
HC1  at  15-20°.  (Fresenius.) 

Nearly  absolutely  insol.  in  alcohol  con- 
taining ether. 

Sol.  in  42,600  pts.  absolute  alcohol.  (Precht, 
Z.  anal.  18.  509.) 

1 1.  methyl  alcohol  dissolves  0.072  g.  at  20°. 
(Peligot,  Monit.  Sci.  1892,  (4)  6.  I,  873.) 

Solubility  in  methyl  alcohol +Aq  at  20°. 


100  pts.  H2O  dissolve  0.926  pt.  at  15  ,  and 
5.26  pts.  at  100°.    (Crookes,  C.  N.  9.  205.) 

100  g.  H2O  dissolve  at: 
2°         16°        25°       35°     48° 
0.4812  0.6718  0.8641  1.132  1.745g.K2PtCl6, 
59°        68°        78°        92° 
2.396     2.913     3.589     4.484  g.  K2PtCl6. 
(Archibald,  J.  Am.  Chem.  Soc.  1908,  30.  752.) 

Not  attacked  by  cold  cone.  H2SO4.     (Las- 
saigne.) 
SI.  sol.  in  cold,  more  easily  in  hot  dil.  acids. 
Less  sol.  in  KCl+Aq  than  in  H2O,  and  nearly 
insol.  in  sat.  KCl+Aq.    (Schrotter,  W.  A.  B. 
50,  2.  268.) 

Solubility  in  KCl+Aq  at  20°. 

%  alcohol  by  wt. 

G.  KoPtCle  in  100  g.  of 
solution 

0 
5 
10 
20 
30 
40 
50 
60 
70 
80 
90 
100 

0.7742 
0.5350 
0.4120 
0.2642 
0.1831 
0.1165 
0.0625 
0.0325 
0.0182 
0.0124 
0.0038 
0.0027 

(Archibald,  J.  Am.  Chem.  Soc.  1908,  30.  755.) 
Solubility  in  ethyl  alcohol  +Aq  at  20°. 

G.  mol.  KC1  per  1.  of 
KC1  +Aq. 

G.  K2PtCl6  in  100  g. 
of  solution. 

%  alcohol  by  wt. 

G.  KzPtCle  in  100  g.  of 
solution 

0.00 
0.20 

0.25 
0.50 
1.00 
2.00 
3.00 
4.00 
sat. 

0.7742 
0.0236 
0.0207 
0.0109 
0.0046 
0.0045 
0.0043 
0.0042 
0.0034 

0 
5 
10 
20 
30 
40 
50 
60 
70 
80 
90 
100 

0.7742 
0.4910 
0.3720 
0.2180 
0.1340 
0.0760 
0.0491 
0.0265 
0.0128 
0.0085 
0,0025 
0.0009 

(Archibald,  J.  Am.  Chem.  Soc.  1908,  30.  757.) 
Solubility  in  NaCl+Aq  at  16°. 

G.  mol.  NaCl  per  litre 
of  NaCl+Aq. 

G.  K2PtCl6  in  100  g. 
of  solution 

(Archibald,  J.  Am.  Chem.  Soc.  1908,  30.  755.) 
Solubility  in  isobutyl  alcohol  +Aq  at  20°. 

0.00 
0.05 
0.10 
0.25 
0.50 
0.75 
1.00 
2.00 

0.672 
0.700 
0.729 
0.758 
0.775 
0.791 
0.805 
0.834 

%  alcohol 

g.  KzPtClein  100  g.  of 
solution 

0 

8.20 
sat. 

0.7742 
0.6250 
0.3180 

(Archibald,  J.  Am.  Chem.  Soc.  1908,  30.  757.) 

(Archibald,  J.  Am.  Chem.  Soc.  1908,  30.  755.) 

242 


CHLOROPLATINATE,  POTASSIUM 


Potassium  pen/achloro/^roplatinate, 

K2(PtCl5OH). 

Easily  sol.  in  H2O.    (Ruff,  B.  1913.     46. 
925.) 

Praseodymium  chloroplatinate,  PrCl3,  PtCl4 

+12H2O. 

Very  sol.  in  H2O.    Sol.  in  cone.  HC1.    (von 
Scheele,  Z.  anorg.  1898,  18.  353.) 

Rubidium  chloroplatinate,  Rb2PtCl6. 

100  pts.  H2O  dissolve  at: 

0°  10°  20° 

0.184  0.154  0.141  pts.  Rb2PtCl6, 

30°  40°  50° 

0.145  0.166  0.203  pts.  Rb2PtCl6; 


60° 
0.253 

90° 
0.521 


70° 
0.329 

100° 
0.634 


80° 
0.417  pts.  Rb?PtCl€, 

pts.  Rb2PtCl6. 


(Bunsen,  Pogg.  113.  337.) 


Sol.  in  740  pts.  H2O  at  15°,  and  157  pts.  at 
100°.    (Crookes,  C.  N.  9.  205.) 
Insol.  in  alcohol. 

Samarium   chloroplatinate,   SmCl3,    PtCl4  + 


Deliquescent.    Very  sol.  in  H2O.     (Cleve, 
Bull.  Soc.  (2)  43.  165.) 

Silver  chloroplatinate,  Ag2PtCl6. 

Ppt.    Gradually  decomp.  by  H2O  into  AgCl 
and  PtCl4.    (Jorgensen,  J.  pr.  (2)  16.  345.) 

Ag2PtCl4(OH)2.    Ppt. 

Silver  mo/iochloroplatinate,  [PtCl(OH)5]Ag2. 
Ppt.     (Bellucci,  Chem.  Soc.  1902,  82.  (2) 
155.) 

Silver  pewtochloroplatinate,  (OH)PtCl5Ag2. 

Ppt.;    stable   in   boiling   H2O.      (Miolati 
Chem.  Soc.  1900,  78  (2).  732.) 

Silver    chloroplatinate    ammonia,    Ag2PtCl6 
2NH3. 

Insol.  in  H2O.    (Birnbaum.) 

Sodium  chloroplatinate,  Na2PtCl6+6H2O. 

Easily  sol.  in  H2O.  Sat.  solution  at  15 
contains  39.77  g.  Na2PtCl6  and  has  sp.  gr 
of  1.368.  Sol.  in  NaCl+Aq.  More  sol.  in 
absolute  alcohol  than  in  95%  alcohol.  Sat 
solution  in  abs.  alcohol  contains  11.90%;  95 <7 
alcohol,  6.34%.  Mixture  of  equal  parts  o 
alcohol  and  ether  dissolve  2.43%.  Insol.  in 
ether.  (Precht,  Z.  anal.  18.  502.) 

Sodium  per^achloroplatinate,  (OH)PtCl5Na; 
Exists  only  in  solution.    (Miolati,  I.e.} 

Strontium  chloroplatinate,  SrPtCls-f  8H2O. 
Very  sol.  in  H2O. 


trontium  raowochloroplatinate,  PtCl(OH)8Sr 

+H20. 

Insol.  in  H2O  and  org.  solvents.    (Bellucci, 
.  C.  1903,  I.  131.) 

Thallium  chloroplatinate,  Tl2PtCl6. 

Very  si.  sol.  in  H2O.     Sol.  in  15,585  pts. 
H2O  at  15°,  and  1948  pts.  at  100°.    (Crookes.) 

Thallium  wo«ochloroplatinate,  [PtCl(OH)  6]T1  . 
Ppt.     (Bellucci,  Chem.  Soc.  1902,  82.  (2). 
55.) 

Thallium  pewtochloroplatinate,  (OH)PtCl5Tl2. 
(Miolati,  Chem.  Soc.  1900,  78  (2).  732.) 

Thorium    chloroplatinate,     ThCl4,     PtCl4-f 

12H2O. 

Very  deliquescent.    (Cleve,  Bull.  Soc.  (2). 
21.  118.) 

Tin  (stannic)  chloroplatinate,  SnCl4,  PtCl4+ 

12H2O. 
(Nilson,  B.  9.  1142.) 

ytterbium  chloroplatinate,  2YbCl3,  PtCl4+ 

22H2O,  and  +35H2O. 
Ppt.    (Cleve,  Z.  anorg.  1902,  32.  137.) 

Vanadyl  chloroplatinate,  (VO)PtCl4  + 


Sol.  in  H2O;  cryst.  from  PtCl4+Aq. 
^Brauner,  M.  3.  58.) 

Yttrium  chloroplatinate,  4YC13,  5PtCl4  + 
52H20. 

Very  deliquescent.    (Cleve.) 

2YC13,  3PtCl4+30H2O.  (Nilson,  B.  9. 
1059.) 

2YC13,  PtCl4+21H2O.    (Nilson.) 

Zinc  chloroplatinate,  ZnPtCl6+6H2O. 
Deliquescent;  sol.  in  H2O  and  alcohol. 

Zinc     tefrachloroplatinate,     ZnPt(OH)2Cl4  + 

5H2O. 

Extremely  sol.  in  H2O  and  alcohol.  (Mio- 
lati, Z.  anorg.  1900,  22.  458.) 

Zirconyl  chloroplatinate,  (ZrO)PtCl6+12H2O. 
(Nilson.) 

Chloroplatinoanhydropf/rophosphoric 


acid,  ClPtP206H4  =  ClPt  '    >  O 

\PO(OH)2. 

Not  deliquescent.    Sol.  in  H2O.    (Schiitzen- 
berger,  Bull.  Soc.  (2)  18.  154.) 

Chloroplatinocyanhydric  acid, 

H2Pt(CN)4Cl2. 
See  Perchloroplatinocyanhydric  acid. 


CHLOROPLATINITE,  MAGNESIUM 


243 


Potassium  chloroplatinocyanide,  5K2Pt(CN)4, 

K2Pt(CN)4Cl2+21H2O. 
Sol.  in  H2O;  insol.  in  alcohol. 

Silver  chloroplatinocyanide, 

Ag2(PtCl2(CN)4)2. 
Ppt.    (Miolati,  C.  C.  1901,  I.  500.) 

Chloroplatinophosphoric  acid, 

Cl2PtP(OH)3. 

Very     deliquescent,     and     sol.     in    H2O. 
(Schiitzenberger,  Bull.  Soc.  (2)  17.  493.) 

Lead  chloroplatinophosphate,  Pb3(Cl2PtPO3)2 
+8H20. 

Ppt. 

Pb3(Cl2PtP03)2,  2PbO+4H20.     Ppt. 
(Schiitzenberger,  Bull.  Soc.  (2)  17.  494.) 

Silver    chloroplatinophosphate,    Ag2HPO3, 

PtCl2. 

Ppt.     (Schutzenberger,  Bull.  Soc.  (2)  17. 
494.) 

ChloroplatinofHphosphoric  acid,  PtCl2, 

P2(OH)6. 

Very  deliquescent,  and  easily  sol.  in  H2O. 
(Schutzenberger,  Bull.  Soc.  (2)  18.  153.) 

Chloroplatino/wrophosphoric  acid. 

^P(OH), 
ClPt'^O 

\P(OH)3. 

Less  deliquescent  than  chloroplatinoGfa'phos- 
phoric  acid. 

Chloroplatinous  acid,  H2PtCl4. 
Known  only  in  solution. 

Aluminum  chloroplatinite,  AlPtCl5+10HH2O. 
Very  deliquescent;  sol.  in  H2O.     (Nilson, 
J.  pr.  (2)  15.  260.) 

Ammonium  chloroplatinite,  (NH4)2PtCl4. 

SI.  sol.  in  cold,  easily  in  hot  H2O.    Insol. 
in  alcohol.    (Peyrone,  A.  55.  206.) 

Barium  chloroplatinite,  BaPtCl4+3H2O. 

Not  deliquescent;  sol.  in  H2O.     Very  si. 
sol.  in  93%  alcohol. 

Cadmium  chloroplatinite  ammonia.  CdPtCl4, 

4NH3. 

Insol.  in  H2O  or  NH4OH+Aq.     Sol.  in 
HCl+Aq.    (Thomsen,  B.  2.  668.) 

Caesium  chloroplatinite,  Cs2PtCl4. 
SI.  sol.  in  cold,  easily  in  hot  H2O. 

100  pts.  H2O  dissolve  3.4  pts.  salt  at  20° 
"  "          6.73  "      "        40° 

"  "          8.68  "      "        60° 

"  "        10.92  "       "        80° 


"        12.10 "       " 
(Godeffroy,  A.  181.  176.) 


100°. 


Cs2PtCl5.  Ppt.  Very  sensitive  to  sun- 
light. Decomp.  by  H2O  into  the  higher  and 
lower  chlorides.  (Wohler,  B.  1909,  42.  4104.) 

Calcium  chloroplatinite,  CaPtCl4+8H2O. 
Deliquescent;  sol.  in  H2O. 

Cerium  chloroplatinite,  CeCl3,  2PtCl2  + 


Deliquescent;  easily  sol.  in  H2O.  (Nilson, 
B.  9.  1847.) 

Chromium     chloroplatinite,     Cr2Pt3Cli2  + 

18H2O. 
Deliquescent. 

Cobalt  chloroplatinite,  CoPtCl4+6H2O. 

SI.  deliquescent  in  moist,  efflorescent  in  dry 
air. 

Copper  chloroplatinite,  CuPtCl4+6H2O. 
Extremely  deliquescent.    (Topsoe.) 

Copper    chloroplatinite    ammonia    (cupram- 

monium  chloroplatinite), 

Cu(NH3)4PtCl4. 

Insol.  in  H2O  or  NH4OH+Aq;  easily  sol. 
in  H2SO4+Aq.  (Millon  and  Commaille,  C.  R. 
57.  822.) 

Didymium  chloroplatinite,   DiCl3,   2PtCl2-f- 

10H2O. 

Deliquescent;  very  sol.  in  H2O.    (Nilson.) 
2DiCl3,  3PtCl2  +  18H2O.    As  above.    (Nil- 

son.) 

Erbium  chloroplatinite,  ErPtCl5+13^H2O. 

Deliquescent. 

Er2Pt3Cli2+24H2O.  Deliquescent  in  moist 
air. 

Glucinum  chloroplatinite,  GlPtCl4+5H2O. 

Deliquescent  in  moist  air.  Sol.  in  H2O  in 
all  proportions. 

Iron     (ferrous)  chloroplatinite,     FePtCl4-f 

7H2O. 

Deliquescent.  Rather  si.  sol.  in  cold,  very 

sol.  in  hot  H2O.  (Nilson.) 

Lanthanum   chloroplatinite,    La2Pt3Cli2+18, 

and  27H2O. 
Deliquescent. 

Lead  chloroplatinite,  PbPtCl4. 
Insol.  in  cold  H2O. 

Lithium  chloroplatinite,  Li2PtCl4+6H2O. 
Sol.  in  H2O. 

Magnesium  chloroplatinite,  MgPtCl4+6H2O. 
Not  very  deliquescent;  very  sol.  in  H2O. 


244 


CHLOROPLATINITE,  MANGANESE 


Manganese  chloroplatinite,  MnPtCl4+6H2O. 
As  the  Mg  salt. 

Mercurous  chloroplatinite. 
Ppt. 

Nickel  chloroplatinite,  NiPtCl4+6H2O. 
As  the  Co  salt. 

Potassium  chloroplatinite,  K2PtCl4. 

Moderately  sol.  in  H2O;  insol.  in  alcohol. 

Rubidium  chloroplatinite,  Rb2PtCl4. 
SI.  sol.  in  colfl;  easily  in  hot  H2O. 

Silver  chloroplatinite,  Ag2PtCl4. 

Insol.  in  H2O.  NH4OH+Aq  dissolves  out 
AgCl.  (Lang.) 

AgCl,  PtCl2(?).  As  above.  (Commaille, 
Bull.  Soc.  (2)  6.  262.) 

Silver    chloroplatinite    ammonia,    Ag2PtCl4, 
4NH3. 

(Thomsen.) 

Sodium  chloroplatinite,  Na2PtCl4-f  4H2O. 
Deliquescent;  very  sol.  in  H2O. 

Strontium  chloroplatinite,  SrPtCl4+6H2O. 
Deliquescent.    Very  sol.  in  H2O. 

Thallium  chloroplatinite,  Tl2PtCl4. 
Very  si.  sol.  even  in  boiling  H2O. 

Thorium  chloroplatinite,  Th2Pt3Cli4-f-24H2O. 
Very  deliquescent. 

Yttrium  chloroplatinite,  Y2Pt3Cli2+24H2O. 
Deliquescent. 

Zinc  chloroplatinite,  ZnPtCl4+6H2O. 

SI.  sol.  in  cold,  more  easily  in  hot  H2O; 
insol.  in  alcohol. 

Zinc   chloroplatinite   ammonia,   ZnPtCl4, 

SI.  sol.  in  H2O;  easily  sol.  in  HCl+Aq. 
Insol.  in  alcohol.  (Thomsen,  J.  B.  1868.  278.) 

Zirconyl  chloroplatinite,  (ZrQ)PtCl4+8H2O. 
(Nilson.) 

Tnchloroplatinous  acid,  H2Pt(OH)Cl3. 

Sol.  in  H2O.  (Miolati,  Z.  anorg.  1902.  33. 
265.) 

+H2O.    (Nilson,  J.  pr.  (2)  15.  260.) 

Lead  fnchloroplatinite,  PbPt(OH)Cl3. 
Ppt.    (Miolati.) 

Silver  fn'chloroplatinite,  Ag2Pt(OH)Cl3. 
Ppt.    (Miolati.) 


Chloroplatosulphurous  acid. 

Ammonium  chloroplatosulphite,  acid, 

NH4PtClSO3,  H2SO3+4H2O. 
Sol.  in  H20.    (Birnbaum,  A.  152.  149.) 

Ammonium  chloroplatosulphite  chloride  sul- 
phite, NH4PtClS03,  (NH4)2S03,  NH4C1. 
Very  deliquescent.    (Birnbaum.) 

Ammonium    chloroplatosulphite    sulphite, 

NH4ClPtS03,  (NH4)2S03+3H20. 
Sol.  in  H2O.    (Birnbaum.) 

Barium     chloroplatosulphite     chloride     am- 
monium    chloride,     Ba(ClPtSO3)2, 
Ba(PtClSO3)Cl,   6NH4C1+3H2O. 
Sol.  in  H2O.    (Birnbaum.) 

Potassium     chloroplatosulphite     ammonium 

chloride,  KPtClSO3,  2NH4C1. 
Very  deliquescent.      (Birnbaum,   A.    152. 

142.) 


e  chloride, 


Potassium  chloroplatosulphit 

KPtClSO3,  2KC1. 
Deliquescent;  sol.  in  H2O.    (Birnbaum,  A. 
152.  145.) 

Potassium     chloroplatosulphite     ammonium 
potassium  sulphite,  KPtClSO3, 
(NH4)KSO3+3H2O. 
Very  deliquescent.     (Birnbaum,   A.    159. 

120.) 

Sodium  chloroplatosulphite  ammonium  chlo- 
ride, NaPtClSO3,  2NH4C1. 
Very  deliquescent.      (Birnbaum,   A.    159. 
117.) 

Chloroplumbic  acid,  H2PbCl6. 

Decomp.  in  solution  on  standing.  (Gut- 
bier,  J.  pr.  1914,  (2)  90.  497.) 

Ammonium  chloroplumbate,  (NH4)2PbCl6. 

Ppt.  Difficultly  sol.  in  a  small  amount  of 
H2O.  Solution  decomp.  slowly  when  cold, 
more  rapidly  when  warmed. 

Decomp.  by  a  large  amount  of  H2O.  Sol. 
without  decomp.  in  20%  HC1.  Decomp.  by 
dil.  acids  and  alkalis.  (Elbs,  Z.  Elektrochem. 
1903,  9.  778.) 

Difficultly  sol.  in  small  amount  of  H20  and 
solution  decomp.  slowly  in  the  cold,  more 
rapidly  when  warmed.  Decomp.  by  a  large 
amount  of  H2O.  (Gutbier,  J.  pr.  1914,  (2) 
90.  498.) 

Sol.  in  cold  HNO3  without  decomp.  (Fried- 
rich,  M.  1893,  14.  511.) 

Insol.  in  cone.  NH4Cl+Aq.  (Nikoljukin, 
B.  18.  370  R.) 

5NH4C1,  2PbCl4.  Not  hygroscopic.  De- 
comp. by  H2O  with  pptn.  of  PbO2.  Sol.  in 
HCl+Aq  and  in  cold  HNO3+Aq  without 


CHLOROPURPUREOCOBALTIC  CHLORIDE 


245 


decomp.    (Classen  and  Zahorski,  Z.  anorg.  4. 
100.) 

Composition  is  2NH4C1,  PbCl4.  (Fried- 
rich,  W.  A.  B.  102,  2b.  527.) 

Caesium  chloroplumbate,  Cs2PbCl6. 

Nearly  absolutely  insol.  in  cone.  CsCl+Aq 
in  presence  of  Cl.  (Wells,  Z.  anorg.  4.  335.) 

1  com.  cone.  HCl+Aq  containing  PbCl4  dis- 
solves 0.000049  g.  Cs2PbCl6.  (Wells,  Z.  anorg. 
4.  341.) 

Reacts  with  H20  as  the  corresponding  am- 
monium salt.  (Gutbier,  J.  pr.  1914,  (2) 
90.  500.) 

Potassium  chloroplumbate,  K2PbCl6. 

Decomp.  by  H20;  sol.  in  KCl+Aq.  (Wells, 
Z.  anorg.  4.  335.) 

Readily  decomp.  in  the  air.  (Gutbier,  J. 
pr.  1914,,  (2)  90.  499.) 

Rubidium  chloroplumbate,  Rb2PbCl6. 

Decomp.  by  H20;  si.  sol.  in  cone.  RbCl  + 
Aq.  (Wells,  Z.  anorg.  4.  335.) 

1  ccm.  cone.  HCl+Aq.  containing  PbCl4 
dissolves  0.003  g.  Rb2PbCls.  (Wells,  Z. 
unorg.  4  341.) 

Reacts  with  H2O  as  the  corresponding  am- 
monium salt.  (Gutbier,  J.  pr.  1914,  (2) 
90.  499.) 

Decomp.  by  cone.  H2SO4.  Insol.  in  96% 
alcohol.  (Erdmann,  A.  1896,  294.  76.) 

Chloropurpureochromium  bromide, 

CrCl(NH3)5Br2. 

Somewhat  more  easily  sol.  in  H2O  than  the 
chloride.  (Jorgensen,  J.  pr.  (2)  20.  105.) 

—  chloride,  CrCl(NH8)6Cl2. 
Difficultly  sol.  in  cold,  and  decomp.  by  hot 

H20. 

1  pt.  dissolves  in  154  pts.  H20  at  16°. 
Insol.  in  cone.  HCl+Aq.  More  sol.  in  dil. 
H2SO4+Aq  than  in  H2O.  Sol.  in  NH4OH  + 
Aq  without  decomp.  (Jorgensen,  J.  pr.  (2)  20. 
105.) 

mercuric    chloride,     CrCl(NH3)6Cl2,   . 

3HgCl2. 
Very  difficultly  sol.  in  H2O.    (Jorgensen.) 

—  chloroplatinate,  CrCl(NH3)5(PtCl6). 
Extremely  difficultly  sol.  in  H2O.    (Jorgen- 
sen.) 

chromate,  CrCl(NH3)6(CrO4). 

SI.  sol.  in  H2O;  si.  more  sol.  than  chloro- 
purpureocobalt  chromate.  (Jorgensen.) 

—  dithionate,  CrCl(NH3)5(S2O6). 

Very  si.  sol.  in  cold,  but  much  more  easily 
in  hot  H2O.  (Jorgensen.) 


Chloropurpureochromium  f  errocyanide. 

[CrCl(NH3)6]2Fe(CN)6+4H20. 
Very  difficultly  sol.  in  cold  H2O.    (Jorgen- 
sen.) 

-  fluosilicate,  CrCl(NH8)6(SiF6). 
Very   difficultly   sol.   in   H2O.     Insol.   in 
H2SiF6+Aq.    (Jorgensen,  J.  pr.  (2)  20.  105.) 

—  mercuric  iodide,  CrCl(NH3)5l2,  2HgI2. 
Decomp.  bv  H20:  sol.  in  alcohol  and  warm 

KCN+Aq.    " 

CrCl(NH3)5I2,  HgI2.  Very  difficultly  sol. 
in  cold  H2O;  easily  sol.  in  KCN+Aq.  (Jor- 
gensen, I.e.) 

—  nitrate,  CrCl(NH3)6(N03)2. 

Sol.  in  71  pts.  H2O  at  17.5°.  Insol.  in 
HNOs+Aq.  (Jorgensen.) 

—  oxalate,  CrCl(NH3)5C2O4. 

Very  si.  sol.  in  cold  H20.    (Jorgensen,  I.e.) 

~  sulphate,  CrCl(NH3)5SO4+2H2O. 
Sol.  in  H2O;  precipitated  by  alcohol.    (Jor- 
gensen.) 

—  sulphate,  acid,[CrCl(NH3)5]4S04(HS04)6. 
Quite  sol.  in  H2O.     (Jorgensen,  J.  pr.  (2) 

20.  185.) 

—  pe^asulphide,  CrCl(NH3)6S5. 

Very  si.  sol.  in  cold,  easily  sol.  in  warm 
H2O.  Decomp.  by  dil.  HCl+Aq.  Insol.  in 
alcohol.  (Jorgensen.) 

Chloropurpureocobaltic  bromide, 

CoCKNH3)6Br2. 

Properties  resemble  the  chloride  very 
closely.  Sol.  in  214  pts.  H2O  at  14.3°  (Jor- 
gensen, J.  pr.  (2)  18.  205.) 

mercuric  bromide, 

4CoCl(NH3)5Br2,  9HgBr2. 

Ppt.    (J.) 

bromoplatinate,  CoCl(NH3)6Br2,  PtBr4. 

Very  si.  sol.  in  H2O.    (J.) 

carbonate,  CoCl(NH3)5CO3+4^H2O. 

Efflorescent;  very  easily  sol.  in  H2O.    (J.) 

chloride,  CoCl(NH3)5Cl2. 

Very  si.  sol.  in  cold,  more  easily  in  hot  H20. 
Sol.  in  244  pts.  H2O  at  15.5°.  (Claudet,  Phil. 
Mag.  J.  (4)  2.  253.)  In  287  pts.  H2O  at  10.2° 
and  255  pts.  at  11.5°.  (Rose,  Pogg.  20.  152.) 
100  pts.  H2O  dissolve  0.232  pt.  CoCl3,  5NH,, 
at  0°,  and  1.031  pts.  at  46.6°.  (Kurnakoff,  J. 
Russ.  Soc.  24.  629.) 

SI.  decomp.  by  cold,  completely  by  boiling 
H2O:  decomp.  prevented  by  a  little  HC1. 
Pptd.  from  aqueous  solution  by  alcohol,  HC1, 


246 


CHLOROPURPUREOCOBALTIC  ANTIMONY  CHLORIDE 


or  sat.  KC1  or  NaCl+Aq;  not  decomp.  by 
boiling  HCl+Aq.  (Claudet,  I.e.]  IN  early 
insol.  in  cold,  but  sol.  in  hot  H2O,  to  which  a 
few  drops  of  HC1  have  been  added.  Less 
sol.  in  dil.  HCl+Aq  than  luteocobaltic  chlor- 
ide. (Rogojski,  A.  ch.  (3)  41.  447.) 
Insol.  in  alcohol.  (Gibbs  and  Genth.) 

Chloropurpureocobaltic    antimony    chloride, 

2CoCl(NH3)5Cl2,  SbCl3. 
Ppt.    Decomp.  by  H2O.    (Gibbs.) 

bismuth  chloride. 

Insol.  in  cone.  HC1.  Easilv  decomp.  by 
H20.  (Gibbs.) 

mercuric  chloride,  CoCl(NH3)5Cl2, 

3HgCl2. 

Insol.  in  cold,  less  sol.  in  hot  H2O  than 
Chloropurpureocobaltic  chloride.  Insol.  in 
cold  fuming  HCl+Aq;  si.  sol.  in  hot  HC1+ 
Aq,  separating  on  cooling;  si.  sol.  in  hot  aqua 
regia;  moderately  sol.  in  hot  HNO3+Aq; 
partly  sol.  in  cold  cone.  H2SO4,  wholly  on 
warming.  Easily  sol.  in  warm  H2C2O4+Aq. 
Insol.  in  HgCl2+Aq. 

Moderately   sol.   in   NH4OH+Aq  or 
(NH4)2CO3+Aq.    (Carstanjen.) 

CoCl(NH3)5Cl2,  2HgCl2.  SI.  sol.  in  cold, 
but  much  more  easily  in  hot  H2O..  (Gibbs, 
Proc.  Am.  Acad.  10.  33.) 

-  chlcropalladite,  CoCl(NH3)5Cl2,  PdCl2. 
SI.  sol.  in  cold,  moderately  sol.  in  hot  H2O. 

(Carstanjen.) 

-  chloroplatinate,  CoCl(NH3)5Cl2,  PtCl4. 
Nearly  insol.  in  cold.    Very  si.  sol.  in  hot 

H2O.    (Gibbs  and  Genth,  Sill.  Am.  J.  (2)  23. 
319.) 

-  chromate,  CoCl(NH3)5CrO4. 
Very  si.  sol.  in  H2O.    (J.) 

-  dichromate,  CoCl(NH3)5Cr207. 

Much  more  easily  sol.  in  H2O  than  the 
neutral  salt.  (J.) 

dithionate,  CoCl(NH3)5S2O6. 

Very  si.  sol.  in  cold,  more  easily  in  hot 
H,0.  (J.) 

manganic  fluoride. 

Ppt.  SI.  sol.  in  dil.  HF+Aq.  (Christen- 
sen,  J.  pr.  (2)  35.  161.) 

—  fluosilicate,  CoCl(NH3)5SiF6. 


Very  si.  sol.  in  HF+Aq. 

-  iodide,  CoCl(NH3)6I2. 

Much  more  sol.  in  H2O  than  bromide  or 
chloride.  Sol.  in  54.5  pts.  H2O  at  15.6°,  and 
50  pts.  at  19.3°.  (J.) 


Chloropurpureocobaltic  mercuric  iodide, 
CoCl(NHs)5I2,  2HgI2. 

SI.  sol.  in  H2O.    (J.) 

CoCl(NH3)5l2,  HgI2.  Verv  si.  sol.  in  cold 
H20.  (J.) 

—  nitrate,  CoCl(NH3)5(NO3)2. 

Sol.  in  80  pts.  H2O  at  15°.  Rather  easily 
sol.  in  hot  H2O.  (Jorgensen,  J.  pr.  (2)  18. 
209.) 

—  oxalate,  CoCl(NH3)5C2O4. 
SI.  sol.  in  H2O.    (J.) 

-  p^/rophosphate,  CoCl(NH3)5(H2P2O7). 

SI.  and  very  slowly  sol.  in  cold,  much  more 
easily  in  warm  H2O.  (J.) 

[CoCl(NH3)5]2P207+zH20.  Quite  easily 
sol.  in  H2O. 

cfo'phosphopentamolybdate, 

[CoCl(NH3)5]2(5MoO3,  2HPO4). 

Ppt.  Nearly  insol.  in  pure  H2O;  more  sol. 
in  dil.  H2SO4+Aq  without  decomp.  (J.) 

[CoCl(NH3)5]2(5MoO3,  2NH4PO4).  Ppt. 
As  above. 

—  sulphate,  CoCl(NH3)6SO4. 
Anhydrous.    Slowly  sol.  in  128-131.9  pts. 

H2O  at  16°. 

+2H2O.  Sol.  in  133.4  pts.  H2O  at  17.3°. 
Rather  easily  sol.  in  hot  H2O,  and  much  more 
rapidly  than  the  anhydrous  salt.  (J.) 

[CoCl(NH3)5]4SO4(SO4H)6.  Decomp.  by 
H2O  into  neutral  sulphate.  Sol.  in  H2SO4. 


tartrate,  CoCl(NH3)5(C4H5O6)2  + 


Moderately  sol.  in  H2O;  insol.  in  alcohol. 

-  thiosulphate,  CoCl(NH3)5S2O3. 
Nearly  insol.  in  cold  H2O;  very  si.  sol.  in 

boiling  H2O  with  partial  decomp.    (J.) 

Chloropurpureoiridium  comps. 
See  Iridopentamine  comps. 

Chloropurpureorhodium  carbonate, 

ClRh(NH3)5CO3+H2O. 
Easily  sol.  in  H2O.    (Jorgensen.) 

-  chloride,  ClRh(NH3)5Cl2. 

Sol.  in  179  pts.  H2O  at  17°,  and  more  easily 
in  hot  H2O.  Sol.  in  cone.  H2SO4  or  boiling 
NaOH+Aq  without  decomp.  Very  si.  sol.  in 
cold  dil.  HCl+Aq  (1  :  1).  SI.  sol.  in  hot  HC1 
+Aq.  Insol.  in  alcohol.  (Jorgensen,  J.  pr. 
(2)  27.  433;  34.  394.) 

-  -  rhodium  chloride, 

3ClRh(NH3)5Cl2,  2RhCl3. 
Ppt.    (Jorgensen,  Z.  anorg.  5.  75.) 


CHLORORUTHENATE,  RUBIDIUM 


247 


Chloropurpureorhodium  chloroplatinate, 

ClRh(NH3)5PtCl6. 
Insol.  in  cold  H2O.    (J.) 

—  fluosilicate,  ClRh(NH3)5SiF6. 

Very  si.  sol.  in  cold  H2O.  Sol.  in  NaOH  + 
Aq  as  roseo  salt.  (J.) 

-hydroxide,  ClRh(NH3)5(OH)2. 
Known  only  in  solution.    (J.) 

—  nitrate,  ClRh(NH3)5(NO3)2. 

SI.  sol.  in  cold  H2O,  but  more  easily  than 
the  chloride.  Sol.  in  boiling  NaOH+Aq  as 
roseo  salt.  (J). 

—  sulphate,  ClRh(NH3)5SO4+2H2O. 
SI.  sol.  in  cold,  more  easily  in  hot  H2O.    (J.) 
4ClRh(NH3)5SO4,  3H2SO4.    SI.  sol.  in  cold, 
more  easily  in  hot  H2O.    (J.) 

Chlororhodous  acid. 

Ammonium  chlororhodite,  (NH4)2RhCl5  + 
B20. 

(Gutbier,  B.  1908,  41.  213.) 

Sol.  in  HoO;  insol.  in  alcohol.  (Wollaston.) 
Not  obtainable.  (Leidie,  A.  ch.  (6)  17.  275.) 

(NH4)3RhCl6+lKH2O.  Sol.  in  H2O,  but 
less  easily  than  Na  salt;  insol.  in  alcohol.  Sol. 
in  dil.  NH4Cl+Aq.  (Glaus,  J.  B.  1865.  423.) 
(Gutbier,  1.  c.) 

Ammonium  chlororhodite  nitrate, 

(NH4)3Rh2Cl6,  2NH4NO3. 
Very  sol.  in  H2O.    Decomp.  by  boiling  with 
H2O.    SI.  sol.  in  HNO3+Aq.    (Leidie,  C.  R. 
107.234.) 

Barium  chlororhodite,  Ba3(RhCl6)2. 

Resembles  the  Na  salt.     (Bunsen,  A.  146. 

276.) 

Caesium  chlororhodite,  Cs2RhCl5+H2O. 

Difficulty  sol.  in  H2O.  (Gutbier,  B.  1908, 
41.  214.) 

Lead  chlororhodite,  Pb3(RhCl6)2. 

Ppt.  Insol.  in  H2O.  (Glaus.)  Not  obtain- 
able. (Leidie.) 

Mercurous  chlororhodite,  Hg3RhGle. 

Ppt.  Insol.  in  H2O.  (Glaus.)  Not  obtain- 
able. (Leidie.) 

Potassium  chlororhodite,  K2RhCl5+H2O. 

Not  efflorescent.  SI.  sol.  in  H2O.  SI.  sol. 
in  KC1— Aq.  (Gibbs.)  Insol.  or  si.  sol.  in 
alcohol.  (Berzelius.) 

Salt  is  anhydrous.    (Leidie.) 

Contains  IHoO.  (Seubert  and  Kobbe,  B. 
23.  2556.) 


Can  be  cryst.  from  H2O  containing  a  little 
HC1.  (Gutbier,  B.  1908,  41.  212. 

K3RhCl6+3H20.  Efflorescent.  SI.  sol.  in 
H2O.  Aqueous  solution  decomp.  to  above  on 
standing.  (Glaus.) 

Not  obtainable.    (Leidie".) 

Also  obtained  by  Seubert  and  Kobbe.  (B. 
23.  2556.) 

.    (Leidie,  C.  R.  111.  106.) 


Rubidium  chlororhodite,  Rb2RhCl6+H2O. 

Difficulty  sol.  in  H2O.  (Gutbier,  B.  1908, 
41,  214. 

Silver  chlororhodite,  Ag3RhCl6. 
Ppt.  Insol.  in  H20.  (Glaus.) 
Not  obtainable.  (Leidie.) 

Sodium  chlororhodite,  Na6Rh,Cl12  +  18H2O. 
Na3RhCl3+9H20. 

Efflorescent.  Sol.  in  1.5  p*ts.  H2O.  Melts 
in  crystal  H2O  at  50°.  Insol.  in  alcohol. 
(Glaus.) 

+12H2O.     (Gutbier,  B.  1908,  41.  213.) 

Chlororuthenic  acid. 

Ammonium  chlororuthenate,  (NH4)2RuCI6. 

Easily  sol.  in  H2O.    (Glaus.) 

Formula  is  (NH4)2Ru(NO)Cl5.  (Joly,  C. 
R,  107.  994.) 

Sol.  in  H2O  with  decomp.  Sol.  in  HC1. 
(Howe,  J.  Am.  Chem.  Soc.  1904,  26.  549.) 

Ammonium  agwochlororuthenate, 

(NH4)2Ru(H2O)Cl5. 
Ppt.    (Howe,  J.  Am.  Chem.  Soc.  1904,  26. 

548.) 

Cassium  chlororuthenate,  Cs2RuCle. 

SI.  sol.  in  H2O.  Sol.  in  hot  dil.  HCl+Aq. 
(Howe,  J.  Am.  Chem.  Soc.  1901,  23.  784.) 

Potassium  chlororuthenate,  K2RuCl6. 

Very  sol.  in  H2O.  Very  si.  sol.  in  cone. 
NH4Cl+Aq.  Insol.  in  70%  alcohol.  (Glaus.) 

Formula  is  K2Ru(NO)Cl5.     (Joly.j 

Very  si.  sol.  in  cold  H2O.  Insol.  in  pres- 
ence of  KC1. 

Partially  decomp.  in  hot  aqueous  solution. 
(Antony,  Gazz.  ch.  it.  1899,  29.  (2),  82.) 

Easily  sol.  in  H2O  with  rapid  decomp. 
Sol.  in  HC1.  (Howe,  J.  Am.  Chem.  Soc. 
1904,  26.  548.) 

Potassium  ag-wochlororuthenate, 

K2Ru(OH2)Gl6. 

Sol.  in  H2O.  (Howe,  J.  Am.  Chem.  Soc. 
1904,  26.  547.) 

Rubidium  chlororuthenate,  Rb2RuCl«. 

SI.  sol.  in  H2O;  sol.  in  hot  dil.  HCl+Aq. 
(Howe,  J.  Am.  Chem.  Soc.  1901,  23.  784.) 


248 


CHLORORUTHENIOUS  ACID 


Chlororuthenious  acid. 

Ammonium  chlororuthenite,  (NH4)4Ru2Clio. 
SI.  sol.  in  H2O.     Insol.  in  NH4Cl+Aq  or 
alcohol.    (Glaus,  J.  pr.  80.  282.) 

Caesium  chlororuthenite,  Cs2RuCl5+H20. 

SI.  sol.  in  H2O;  sol.  in  HCl+Aq.    (Howe, 
J.  Am.  Chem.  Soc.  1901,  23.  785.) 

Potassium   cblororuthenite,    K4Ru2Cli9. 

Moderately  sol.  in  cold,  more  easily  in  hot 
H2O.    Decomp.  easily  by  heating.    Insol.  in 


ng. 

% 


cone.  NH4Cl-f  Aq.    Insol.  in  80%  alcohol. 

Rubidium  chlororuthenite,  Rb2RuCl6+H20. 
SI.  sol.  in  H2O;  sol.  in  HCl+Aq.    (Howe, 
J.  Am.  Chem.  Soc.  1901,  23.  786.) 

Sodium  chlororuthenite,  Na4Ru2Clio. 
Deliquescent*   Sol.  in  H2O  or  alcohol. 

Tn'chlorosilicomercaptane. 
See  Silicon  chlcrohydrosulphide. 

Chlorosmic  acid. 

Ammonium  chlorosmate,  (NH4)2OsCl6. 

SI.  sol.  in  H20.    Insol.  in  alcohol  and  H2O 
containing  HC1. 

Potassium  chlorosmate,  K2OsCl6. 
Properties  as  the  NH4  salt. 

Potassium  amino  chlorosmate, 

(NH2)OsCl3,2KCl. 
Ppt.     (Brizard,  A.  ch.  1900,  (7)  21.  375.) 

Potassium     amino,    chlorosmate     hydrogen 

Chloride,  (NH2)CsGl3,2KCl,HCl. 
Ppt.    (Brizard,  A.  ch.  1900,  (7)  21.  378.) 

Silver  chlorosmate,  Ag2OsCl6. 

Irspl.  in  H2O  or  HNO3-j-Aq.     (Claus  and 
Jacoby.) 

Silver  chlorosmate  ammonia,  Ag2OsCl6,  2NH8. 
Sol.  in  much  H2O.    SI.  sol.  in  KOH+Aq. 
Easily  sol.  in  KCN+Aq.    (C.andJ.) 

Sodium  chlorosmate,  Na2OsCl6+2H20. 
Easily  sol.  in  H2O  or  alcohol. 

Chlorosmious  acid. 

Ammonium  chlorosmite, 

(NH4)4Os2Cl10+3H2O. 
Easily  sol.  in  H2O  and  alcohol;  insol.  in 
•ether.    (Claus  and  Jacoby,  J.  pr.  90.  65.) 

Potassium  chlorosmite,  K6Os2Cl12+6H2O. 

Very  easily  sol.  in  H2O  or  alcohol.    Insol. 
in  ether.    (C.  and  J.) 


Chlorosmisulphurous  acid. 

Potassium  hydrogen  chlorosmisulphite, 

OsCl4(SO3)4K6H2. 

Ppt.    (Rosenheim,  Z.  anorg.  190Q,  24.  422.) 

Sodium  chlorosmisulphite, 

OsCl2(SO3)4Na6+10H2O. 


Ppt, 
420.) 


(Rosenheim,    Z.    anorg.    1900,    24. 


Chloropi/roselenious  acid. 

Ammonium    chloropz/roselenite,    NH4C1, 

2SeO2+2H2O. 

Sol.  in  H2O.  (Muthmann  and  Schafer,  B. 
26.  1008.) 

Potassium  chloropyroselenite,  KC1,  2SeO2  + 

H2O. 
AsNH4salt.    (M.andS.) 

Rubidium    chlorop^/roselenite,    RbCl, 

2SeO2+2H2O. 
As  NH4  salt.    (M.  and  S.) 

Chlorostannic  acid,  SnO(OH)Cl. 

(Mallet,  Chem.  Soc.  35.  524.) 

H2SnCl6+6H2O.  Extremely  deliquescent; 
sol.  in  H2O.  (Seubert,  B.  20.  793.) 

Ammonium     chlorostannate,     (NH4)2SnCl6 

(pink  salt). 

Sol.  in  3  pts.  H2O  at  14.5°.  Solution  de- 
comp.  on  boiling  when  dilute,  but  not  when 
cone.  (Bolley.) 

Barium  chlorostannate,  BaSnCle+5H2O. 
Sol.  in  H2O.    (Lewy,  A.  ch.  (3)  16.  308.) 

Caesium  chlorostannate,  Cs2SnCle. 

Nearly  insol.  in  cone.  HCl+Aq.  (Sharp- 
ies, Sill.  Am.  J.  (2)  47.  178.) 

Calcium  chlorostannate,  CaSnCl6+5H2O. 

Very  deliquescent.  (Lewy,  A.  ch.  (3)  16. 
308.) 

Cerium    chlorostannate,    CeSnCl7+9H2O. 

Deliquescent.  Sol.  in  H2O.  (Cleve,  Bull . 
Soc.  (2)  31.  197.) 

Cobalt  chlorostannate,  CoSnCl6+6H2O. 
Sol.  in  H2O.    (Jorgensen.) 

Didymium   chlorostannate,    DiCl3,    SnCl4+ 

10^H20. 
Sol.  in  H2O.    (Cleve.) 

Glucinum  chlorostannate,  GlSnCl6+8H2O. 

Deliquescent.  Sol.  in  H2O.  (Atterberg, 
Sv.  V.  A.  Handl.  12.  No.  4.  14.) 


CHLOROTELLURATE,  RUBIDIUM 


249 


Lanthanum  chlorostannate,  4LaCl3,  5SnCl4+ 

45H2O. 
Deliquescent.    Sol.  in  H2O.    (Cleve.) 

Lithium  chlorostannate,  Li2SnCl6+8H2O. 

Sol.  in  little  H2O  without  decomp.,  but 
decomp.  by  dilution.  (Chassevant,  A.  ch.  (6) 
30.  42.) 

Magnesium  chlorostannate,  MgSnCl6+6H2O. 
Very  deliquescent.    (Lewy.) 

Manganous  chlorostannate,  MnSnCl6+6H2O. 
Deliquescent  in  moist,  efflorescent  in  dry 
air.    (Jorgensen.) 

Nickel  chlorostannate,  NiSnCl6+6H2O. 
Sol.  in  H2O.     (Jorgensen.) 

Potassium  chlorostannate,  K2SnCl6. 
Sol.  in  H2O. 

Sodium  chlorostannate,  Na2SnCl6+6H2O. 

Easily  sol.  in  H2O.  (Topsoe,  Gm.  K. 
Handb.  6te  aufl.  III.  149.) 

Strontium  chlorostannate,  SrSnCl6+8H20. 

SI.  deliquescent,  and  easily  sol.  in  H2O. 
(Topsoe.) 

Yttrium  chlorostannate,  YC13,  SnCl4+8H20. 
Sol.  in  H2O.    (Cleve,  Bull.  Soc.  (2)  31.197.) 

Zinc  chlorostannate,  ZnSnCl6+6H2O. 
(Biron,  C.  C.  1904,  II.  410.) 

Chlorosulphobismuthous  acid. 

Cuprous    chlorosulphobismuthite, 
2Cu2S,  Bi2S3,  2BiSCl. 

Stable  in  air  and  insol.  in  H2O  at  ord. 
temp. 

Decomp.  by  boiling  H20. 

Decomp.  by  mineral  acids  with  evolution 
of  H2S.  (Ducatte,  C.  R.  1902,  134.  1212.) 

Lead    chlorosulphobismuthite,    PbS,    Bi2S3, 
2BiSCl. 

Stable  in  the  air.  Insol.  in  H2O;  decomp. 
by  boiling  H2O;  sol.  in  dil.  acids  with  de- 
comp. and  evolution  of  H2S.  (Ducatte.) 

Chlorosulphonic  acid,  HC1S03. 
See  Sulphuryl  hydroxyl  chloride. 

Chloropi/rosulphonic  acid. 

Ammonium  chlorop^/rosulphonate, 
C1S2O6NH4. 

Fumes  in  the  air. 

Decomp.  by  H2O  and  alcohol.  (Traube, 
B.  1913,  46.  2519.) 


Sodium  chloropi/rosulphonate,  ClS2O6Na. 
Fumes  in  the  air. 
Decomp.  by  H2O  and  alcohol.     (Traube.) 

Chlorosulphuric  acid,  HS08C1. 
See  Sulphuryl  hydroxyl  chloride. 
SO2C12.    See  Sulphuryl  chloride. 

Aluminum  chlorosulphate,  A1(SO4)C1+6H2O. 
Very  sol.  in  H2O.     Nearly  insol.  in  abs. 
alcohol.     (Recoura,  Bull.  Soc.  1902,  (3)  27. 
1155.) 

Chromium  chlorosulphate,  CrClSO4+5H2O. 

Green.  (Weinland,  Z.  anorg.  1905,  48. 253.) 
(Recoura,  C.  R.  1902,  135.  164.) 

Violet.  (Weinland,  Z.  anorg.  1905,  48. 
254.) 

Very  sol.  in  H2O.  Insol.  in  a  mixture  of 
alcohol  and  acetone.  (Recoura,  C.  R.  1902, 
135.  164.) 

+8H2O.    Two  isomeric  modifications: 

(a)  Green   needles.     Easily   sol.    in   H2O. 
(Weinland,  Z.  anorg:  1906,  48.  251.) 

(b)  Violet    plates.     Easily   sol.    in    H2O. 
(Weinland.) 

Chlorosulphurous  acid. 

Ammonium  palladious  tfnchlorosulphite, 

(NH4)3PdCl3S03+H2O. 
Easily  sol.  in  H20.    (Rosenheim,  Z.  anorg. 
1900,  23.  30. 

Chlorotelluric  acid. 

Ammonium  chlorotellurate,  (NH4)2TeCl6. 

Sol.  without  decomp.  in  a  small  amt.  of 
H2O,  but  decomp.  by  much  H2O  or  alcohol. 

Caesium  chlorotellurate,  Cs2TeCl6. 

Decomp.  by  H2O.    Sol.  in  dil.  HCl+Aq. 

100  pts.  HCl+Aq  (sp.  gr.  1.2)  dissolve  0.05 
pt.  at  22°. 

100  pts.  HCl+Aq  (sp.  gr.  1.05)  dissolve 
0.78  pt.  at  22°. 

Insol.  in  alcohol.  (Wheeler,  Sill.  Am.  J. 
145.  267.) 

Potassium  chlorotellurate,  K2TeCl6. 

Deliquescent;  decomp.  by  H2O  and  abso- 
lute alcohol.  (Berzelius.) 

The  most  sol.  in  H2O  of  the  chloro-  or 
bromo-tellurates.  Easily  sol.  in  dil.  HC1 + Aq; 
cone.  HCl+Aq  ppts.  KC1.  (Wheeler,  Sill. 
Am.  J.  145.  267.) 

Rubidium  chlorotellurate,  Rb2TeCl6. 

Decomp.  by  H2O.  Much  more  sol.  in  dil. 
HCl+Aq  than  Cs2TeTl6. 

100  pts.  HCl+Aq  (sp.  gr.  1.2)  dissolve  0.34 
pt.  at  22°. 

100  pts.  HCl+Aq  (sp.  gr.  1.05)  dissolve, 
13.99  pts.  at  22°. 

SI.  sol.  in  alcohol.    (Wheeler.) 


250 


CHLOROTETRAMINE  CHROMIUM  BROMIDE 


Chlorotetramine  chromium  bromide, 

ClCr(NH3)4(OH2)Br2. 
Very   easily  sol.   in   H2O.     (Cleve,   1861, 
(Jorgensen,  j".  pr.  (2)  42.  210.) 

—chloride,  ClCr(NH3)4(OH2)Cl2. 

Sol.  in  H2O,  but  decomp.  by  boiling.  Sol. 
in  HCl+Aq,  and  this  solution  may  be  boiled 
without  decomp.  (Cleve.) 

Sol.  in  15.7  pts.  H2O  at  15°.  (Jorgensen,  J. 
pr.  42.  208.) 

chromate,   ClCr(NH3)4(OH2)CrO4. 

Precipitate.     (Cleve.) 

fluosilicate,  ClCr(NH3)4(OH2)SiF6. 

SI.  sol.  in  H2O.     (Jorgensen,  J.  pr.  (2)  42. 

218.) 

-  hydroxide,  ClCr(NH3)4(OH)2. 
Known  only  in  solution.     (Cleve.) 

—  iodide,  ClCr(NH3)4(OH2)I2. 


Easily  sol.  in  H2O.    (Cleve.) 

-  nitrate,  ClCr(NH3)4(OH2)(NO3)2. 
Very  easily  sol. in  H2O.    (Cleve);  (Jorgen- 
sen, J.  pr.  (2)  42.  209.) 

-  sulphate,    ClCr(NH3)4(OH2)SO4. 
Very  difficulty  sol.  in  cold,  more  easily  in 

hotH2O.    (Cleve.) 

Chlorotetramine  cobaltic  bromide, 

ClCo(NH3)4(OH2)Br2. 
More  sol.  in  H2O  than  chloride.     Nearly 
insol.  in  HBr+Aq/l:l).      (Jorgensen,  J.  pr. 
(2)  42.  215.) 

-  chloride,  ClCo(NH3)4(OH2)Cl2. 

Sol.  in  about  40  pts.  H2O,  and  is  identical 
with  octamine  cobaltic  purpureochloride  of 
Vortmann.  (Jorgensen,  J.  pr.  (2)  42.  211.) 


chloroplatinate,  ClCo(NH3)4(OH,)PtCl6 

+2H20. 
SI.  sol.  in  H2O.    (Jorgensen.) 

-  chromate,  ClCo(NH3)4(OH2)CrO4. 
Easily  sol.  in  cold  H2O.    (Jorgensen,  J.  pr. 

.(2)42.216.) 

-  fluosilicate,  ClCo(NH3)4(OH2)SiF6. 

SI.  sol.  in  H2O.    Nearly  insol.  in  H2SiF6+ 
Aq.     (Jorgensen,  J.  pr.  (2)  42.  219.) 

-  sulphate,  ClCo(NH3)4(OH2)SO4. 

Sol.  in  H2O.    (Jorgensen,  J.  pr.  (2)  42.  214.) 

Chlorotitanic  acid,    TiCl4,2HCl  =  H2TiCl6. 

Known  only  in   solution.      (Kowalewsky, 
Z.  anorg.  1900,  25.  192.) 


Chlorous  acid,  HC102. 

Known  only  in  aqueous  solution.  100  g. 
H2O  at  8.5°  and  753  mm.  pressure  dissolve 
4.7  g.  C12O3.  Hydrate  with  50.07-67.43% 
H2O,  perhaps  HC1O2+H2O,  separates  out 
at  0°.  (Brandan,  A.  151.  340.) 

Pure  HC1O2  is  not  known  even  in  solution. 
(Garzarolli-Thurnlakh,  A.  209.  184.) 

Chlorites. 

All  chlorites  are  'easily  sol.  in  H2O  and 
alcohol,  with  gradual  decomp. 

Ammonium  chlorite. 

Known  only  in  aqueous  solution,  which 
decomposes  on  evaporation  or  long  standing. 

Barium  chlorite,  Ba(ClO2)2. 

Deliquescent;  easily  sol.  in  H2O.  Solu- 
tion decomp.  on  evaporation.  Easily  sol.  in 
alcohol.  (Millon,  A.  ch.  (3)  7.  298.) 

Lead  chlorite,  Pb(ClO2)2. 

Nearly  insol.  in  cold  H2O,  and  only  si.  sol. 
in  hot  H2O.  Sol.  in  KOH+Aq.  (Garzarolli 
and  Hayn,  A.  209.  203.) 

Lead    chlorite    chloride,   6Pb(ClO,)2,4PbCl2, 

PbO. 

Rather  difficulty  sol.  in  H2O.  (Schiel,  A. 
109.  317.) 

Potassium  chlorite,  KC1O2. 

Very  deliquescent  and  sol.  in  H2O.  Sol.  in 
alcohol  of  38°.  (Millon,  A.  ch.  (3)  7.  323.) 

Sol.  in  HClO2+Aq. 

Silver  chlorite,  AgClC2. 

Sol.  in  hot,  less  in  cold  H2O.  Easily  de- 
comp. bv  heating  above '100C.  Decomp.  by 
weakest  acids.  (Millon,  A.  ch.  (3)  7.  329.) 

Sodium  chlorite,  NaClO2. 

Very  deliquescent,  and  sol.  in  H2O. 

Strontium  chlorite,  Sr(ClO2)2. 

Deliquescent  and  sol.  in  H2O.  Decomp.  by 
slow  evaporation.  (Millon,  A.  ch.  (3)  7.  327.) 

Chloroxyfulminoplatinum, 

Pt4N4Cl(OH)O12H22. 

Insol.  in  H2O ;  sol.  in  HCl+Aq.  (v.  Meyer, 
J.  pr.  (2)  18.  305.) 

Chloruranic  acid,  HUO3C1+2H2O. 

Sol.  in  H2O;  si.  sol.  in  alcohol.  (Mylius,  B. 
1901,  34.  2776.) 

Chromacichloride,  CrO2Cl2. 
See  Chromyl  chloride. 

)hromatoiodic  acid. 
See  Chromoiodic  acid. 


CHROMATE,  AMMONIUM  CHROMYL 


251 


Chromic  acid,  H2CrO4. 

Very  sol.  in  H2O.  (Moissan,  C.  R.  98. 
1851.) 

Does  not  exist  except  in  solution.  (Field, 
Chem.  Soc.  61.  405.) 

The  composition  of  the  hydrates  formed  by 
H2CrO4  at  different  dilutions  is  calculated 
from  determinations  of  the  lowering  of  the 
fr-pt.  produced  by  H2CrO4  and  of  the  con- 
ductivity and  sp.  gr.  of  H2CrO4+Aq.  (Jones, 
Am.  Ch.  J.  1905,  34.  333.) 

See  also  Chromium  ^noxide. 

Chromates. 

Chromates  of  the  alkali  metals  and  of  Ca, 
Mg,  and  Sr  are  sol.  in  H2C;  the  others  are 
generally  insol.  or  si.  sol.  in  H2O,  but  sol.  in 
HNOs+Aq. 

Aluminum  chromate,  basic,  A12O3,  CrO3  + 
7H20. 

Easily  sol.  in  NH4OH+Aq,  alum,  or  acetic 
acid+Aq.  Insol.  in  NH4Cl+Aq.  (Farrie, 
Chem.  Soc.  4.  300.) 

Insol.  as  such  as  H2O,  but  easily  decomp. 
into  H2CrO4  and  a  basic  insol.  comp.  Sol.  in 
alkaline  solutions  and  acids.  Decomp.  by 
many  salts.  (Eliot  and  Storer,  Proc.  Am. 
Acad.  5.  214.) 

Aluminum  sodium  chromate  silicate, 

4Al2O3,5Na2O,CrO3,7SiO2. 
(Weyberg,  C.  B.  Miner,  1904.  727.) 

Ammonium     chromate,     basic,     5(NH4)2O, 

4Ci03(?). 

Easily  sol.  in  cold  H2O.  (Pohl,  W.  A.  B. 
6.  592.) 

Ammonium  chromate,  (NH4)2CrO4. 

Very  sol.  in  H2O;  pptd.  from  aqueous  solu- 
tion by  alcohol.  (Malaguti  and  Sarzeau.) 

100  g.  H2O  dissolve  40.46  g.  at  30°. 
(Schreinemakers,  Chem.  Weekbl.  1905,  1. 
395.) 

Sol.  in  H2O  without  decomp.  ( Schreine- 
makers, C.  C.  1905,  II.  1067.) 

Sp.  gr.  of  (NH4)2CrO4+Aq  at  t°/4°. 
t°  13°        13.7°         19.6° 

%  (NH4)2CrO4      10.52         19.75        28.04 
Sp.  gr.  1.0633       1.1197       1.1727 

(Slotte,  W.  Ann.  1881,  14.  18.) 

SI.  sol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  826.) 

Difficulty  sol.  in  acetone.  (Naumann, 
B.  1904,  37.  4328.) 

Ammonium  ^chromate,  (NH4)2Cr2O7. 

Less   sol.    in   H2O    than    (NH4)2CrO4. 
(Moser.)     . 

100    g.     H2O     dissolve     47.17g     at     30°. 


(Schreinemakers,    Chem.    Weekbl.    1905,    1. 
395.) 

Sp.  gr.  of  (NH4)2Cr2O7+Aq  at  t°/4°. 
t°  12°        10.5°  12° 

%  (NH4)2Cr2O7       6.85         13.00         19.93 
Sp.  gr.  1.0393       1.0782       1.1258 

(Slotte,  W.  Ann.  1881,  14.  18.) 

Sol.  in  alcohol.  (Ranitzer,  Zeit.  angew 
ch.  1913,  26.  456.) 

Insol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1370.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

Ammonium  Jn'chromate,  (NH4)2Cr3Oi0. 

Not  deliquescent,  but  very  sol.  in  H2O. 
(Siewert.) 

Decomp.  by  H2O  into  chromic  acid  and 
dichromate.  (Jager  and  Kriiss,  B.  22.  2036.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

Ammonium  te/rachromate,  (NH4)2Cr4Oi3. 

Deliquescent.  Decomp.  bv  H2O.  (Jager 
and  Kriiss,  B.  22.  2037.) 

Ammonium  hexachromate.  (NH4)2CrBOi9  + 
10H2O  (?) 

Very  efflorescent.  (Rammelsberg,  Pogg. 
94.  516.) 

Ammonium  barium  chromate, 

BaCrO4,(NH4)2CrO4. 

Ppt.  Decomp.  by  H2O.  (Groger,  Z. 
anorg.  1908,  58.  414.) 

Ammonium    cadmium    chromate,    (NH4)2O, 

4CdO,  4CrO3+3H2O. 

Ppt.  Decomp.  by  boiling  II2O.  (Groger, 
M.  1904,  25.  533. 

Ammonium  cadmium  chromate  ammonia, 
(NH4)  2CrO4,CdCrO4,  ^NH3  + 1  ^H2O . 

Decomp.  by  H2O.  (Groger,  Z.  anorg.  1908, 
58.  418.) 

(NH4)2Cd(CrO4)2,  2NHS.  Insol.  in  cold, 
decomp.  by  hot  H2O. 

Sol.  in  dil.  acids  or  in  NH4OH+Aq. 
(Briggs,  Chem.  Soc.  1903,  83.  395.) 

Ammonium  chromous  chromate (?), 

(NH4)2Cr04,CrCrO4  =  (NH4)2Cr(CrO4)2. 
Difficultly  sol.  in  H2O.  Insol.  in  alcohol, 
ether,  chloroform,  or  glacial  acetic  acid. 
Easily  sol.  in  cone,  acids,  from  which  it  is 
separated  on  dilution.  Decomp.  by  NaOH-|- 
Aq.  (Heintze,  J.  pr.  (2)  4.  220.)  * 

Ammonium  chromyl  chromate,    i3(NH4)2O, 

2CrO2,3CrO3. 

Nearly  insol.  in  H2O.  (Pascal,  C.  R.  1909, 
148.  1465.) 


252 


CHROMATE,  AMMONIUM  COBALTOUS 


Ammonium  cobaltous  chromate. 

(NH4)2Co(CrO4)2+6H2O. 
Ppt.     Easily  decomp.     (Briggs,  Z.  anorg. 

1907,  66.  247.) 

(NH4)2O,  4CoO,  4CrO3+3H2O.  Insol.  in 
H2O.  Sol.  in  cold  dil.  H2SO4.  (Groger,  Z. 
anorg.  1906,  49.  202.) 

Ammonium   cobaltous   bichromate, 

CoCr207,(NH4)2Cr2O7+2H2O. 
SI.  hydroscopic;  sol.  in  H2O,  insol.  in  al- 
cohol.    (Kruss,  Z.  anorg.  1895,  8.  454.) 

Ammonium  cobaltous    chromate   ammonia, 

3CoCrO4,(NH4)2CrO4,  2NH3+3H2O. 
Ppt.;  decomp.  by  H2O.    (Groger,  Z.  anorg. 

1908,  58.  422.) 

Ammonium    cupric    bichromate, 

2CrCr207,3(NH4)2Cr207+6H20. 
Sol.  in  H2O.     (Kruss,  Z.  anorg.  1895,  8. 
455.) 

Ammonium  cupric  chromate  ammonia, 
(NH4)2CrO4,CuCrO4,2NH3. 

Decomp.  by  H2O.  (Groger,  Z.  anorg. 
1908,  68.  420.) 

Insol.  in  cold,  decomp.  by  hot  H2O.  Sol. 
in  dil.  acids  or  in  NH4OH+Aq.  (Briggs, 
Chem.  Soc.  1903,  83.  394.) 

Ammonium    iron    (ferric)    chromate, 
(NH4)2CrO4,Fe2(CrO4)3+4H2O. 

More  easily  decomp.  by  H2O  than  K2CrO4, 
Fe2(CrO4)3+4H2O.  (Hensgen,  B.  12.  1300.) 

6CrO3,  5Fe2O3,  6(NH4)2O,  and  4CrO8, 
Fe2O3,(NH4)2O+4H2O.    Ppts.    (Lepierre,  C. 
R.  1894,  119.  1217.) 

Ammonium  lithium  chromate,  NH4LiCrO4-f 

2H20. 
Not  deliquescent.     (Rammelsberg.) 

Ammonium    lead    chromate.     (NH4)2CrO4, 

PbCr04. 

Ppt.  Decomp.  by  H2O.  (Groger,  Z. 
anorg.  1908,  58.  424.) 

Ammonium  magnesium   chromate, 
(NH4)2Cr04,  MgCr04+6H20. 

Much  more  sol.  in  HaO  than  the  correspond- 
ing sulphate,  (v.  Hauer.) 

Sol.  in  H2O.  (Groger,  Z.  anorg.  1908,  58. 
416.) 

Ammonium    manganous     chromate, 

(NH4)2CrO4,  2MnCrO4. 
Sol.  in  H2O.    (Hensgen,  R.  t.  c.  3.  433.) 

Ammonium  nickel  chromate,  (NH4)2CrO4, 
NiCrO4+6H2O. 

Sol.  in  H2O.  (Groger,  Z.  anorg.  1906,  51. 
353.) 


Can  be  cryst.  from  H2O  under  40°.  (Briggs, 
Chem.  Soc.  1903,  83.  392.) 

Ammonium    nickel    chromate    ammonia, 
(NH4)2CrO4,NiCrO4,NH3+H2O. 

Decomp.  by  H2O.  (Groger,  Z.  anorg. 
1906,  51.  354.) 

(NH4)2Ni(CrO4)2,  2NH3.  Insol.  in  cold 
H2O.  Decomp.  by  hot  H2O.  Sol.  in  dil. 
acids  or  in  NH4OH+Aq.  .(Briggs,  Chem. 
Soc.  1903,  83.  393.) 

+6H2O.  (Briggs,  Proc.  Chem.  Soc.  1902, 
18.  254.) 

Ammonium  potassium  chromate,  NH4KCr04. 
Sol.  in  H2O.     (E.  Kopp,  C.  N.  11.  16.) 
+H2O.    (Etard,  C.  R.  85.  443.) 
2(NH4)2CrO4,  3K2CrO4.    Very  sol.  in  H2O. 

(Zehenter,  M.  1897,  18.  51.) 

Ammonium    silver    chromate,    (NH4)2CrO4, 

3Ag2CrO4. 

Decomp.  by  H2O.  (Groger,  Z.  anorg. 
1908,  58.  423.) 

Ammonium  sodium  chromate,  NH4NaCrO4+ 

2H2O. 

Very  sol.  in  H2O.  (Zehenter,  M.  1897,  18. 
54.)  ' 

Ammonium  strontium  chromate,  (NH4)2CrO4, 

SrCrO4. 

Ppt.  Decomp.  by  H2O.  (Groger,  Z. 
anorg.  1P08,  58.  415.) 

Ammonium  uranyl  chromate,  (NH4)2CrO4, 
2(UO2)CrO4+6H2O. 

Decomp.  by  boiling  with  H2O.  Sol.  in 
acidulated  H2O.  (Formanek,  A.  257,  106.) 

+3H2O.     (Formanek.) 

Ammonium  zinc  chromate,    (NH4)2O,  2ZnO, 

2Cr03+H2O. 

Decomp.  by  hot  H2O.  (Groger,  M.  1904, 
25.  520.) 

Ammonium    zinc    chromate    ammonia, 
(NH4)2Zn(Cr04)2,  2NH3. 

Insol.  in  cold,  decomp.  by  hot  H2O.    Sol. 
in  dil.  acids  or  in  NH4OH+Aq.     (Briggs,, 
Chem.  Soc.  1903,  83.  394.) 

4ZnCrO4,  2(NH4)2CrO4,  3NH3+3H2O. 
Ppt.    Decomp.  by  H2O.    (Groger,  Z.  .anorg. 
1908,  58.  416.) 

Ammonium    bichromate    chloride    mercuric 
chloride,  (NH4)2Cr2O7,2NH4Cl,4HgCl2  + 
2H2O. 
Ppt.    Sol.  in  cold,  more  sol.  in  warm  H20. 

(Stromholm,  Z.  anorg.  1912,  76.  280.) 

Ammonium    bichromate    chloride    mercuric 
cyanide,     (NH4)2Cr2O7,    4NH4C1, 
6Hg(CN)2+4H20. 
(Stromholm,  Z.  anorg.  1913,  80.  157.) 


CHROMATE,  BISMUTH,  BASIC 


253 


Ammonium    chromate    chromyl    fluoride, 

(NH4)2CrO4,  CrO2F2. 
Sol.  in  H2O.    (Varenne,  C.  R.  91.  989.) 

Ammonium  chromate  iodate. 
See  Chromoiodate,  ammonium. 

Ammonium   cfa'chromate   mercuric   chloride. 

(NH4)2Cr207,  HgCl2. 

Cannot  be  recryst,  from  H2O  or  HgCl2+Aq, 
but  from  (NH4)2Cr2O7+Aq.  (Jager  and 
Kriiss,  B.  22.  2044.) 

+H2O.  (Richmond  and  Abel,  Chem.  Soc. 
Q.  J.  3.  199.) 

Cannot  be  made  to  crystallize  with  H2O. 
(Jager  and  Kriiss.) 

3(NH4)2Cr2O7,  HgCl2.  Decomp.  by  H2O. 
(J.  and  K.) 

4(NH4)2Cr2O7,  HgCl2.  Decomp.  by  H2O. 
(J.  and  K.) 

(NH4)2Cr2O7,  3HgCl2.    (J.  and  K.)      ' 

(NH4)2Cr2O7,  4HgCl2.    (J.  and  K.) 

Ammonium  chromate  phosphate. 
See  Phosphochromate,  ammonium. 

Ammonium  chromate  tellurate. 
See  Chromotellurate,  ammonium. 

Barium  chromate,  BaCrO4. 

Extremely  si.  sol.  in  HaO. 

Calculated  from  electrical  conductivity  of 
BaCrO4+Aq,  1  1.  H2O  dissolves  3.8  *mg. 
BaCrO4  at  18°.  (Kohlrausch  and  Rose,  Z. 
phys.  Ch.  12.  241.) 

When  not  ignited,  BaCrO4  is  sol.  in  86,957 
pts.  H20;  22,988  pts.  NH4Cl+Aq  (0.5% 
NH4C1);  3670  pts.  HC2H3O2+Aq  (5% 
HC2H3O2);  1986  pts.  HC2H302+Aq  (10% 
HC2H3O2);  1813  pts.  H2CrO4+Aq(10% 
CrUa).  When  ignited,  160,000  pts.  H2O  are 
necessary  for  solution.  (Schweitzer,  by  Fre- 
senius,  Z.  anal.  29.  414.) 

Sol.  in  23,000  pts.  boiling  H2O.  (Mescher- 
zerski,  Z.  anal.  21.  399.) 

3.5  mg.  BaCr04  are  dissolved  in  1  1.  of  sat. 
solution  at  18r.  (Kohlrausch,  Z.  phys.  Ch. 
1908,  64.  168.) 

Easily  sol.  in  HNO3,HC1,  or  chromic  acid  + 
Aq,  from  which  it  is  precipitated  by  NH4OH, 
or  by  dilution  with  H2O.  (Bahr.) 

Insol.  in  K2Cr2O7+Aq.     (Schweitzer.) 

Sol.  in  4P.381  pts.  NH4C2H3O2+Aq  (0.75 
%  salt)  at  15°;  in  23,355  pts.  NH4C2H3O2+Aq 
(1.5%  salt)  at  15°;  in  45,162  pts.  NH4N03 
+Aq  (0.5%  salt)  at  15°.  (Fresenius,  Z.  anal. 
29.  418.) 

Easily  sol.  in  alkali  tartrates,  or  citrates  + 
Aq.  (Fleischer,  J.  pr.  (2)  6.  326.) 

C.22X10-4  g.  equiv.  BaCrO4  are  dissolved 
in  1 1.  of  45%  alcohol  at  ord.  temp.  (Guerini, 
Dissert,  1912.) 

Insol.  in  acetic  acid  and  in  M2Cr2O7+Aq. 

Partly  sol.  in  a  mixture  of  the  two,  except 


in  presence  of  MC2H3O2.  (Caron  and  Raquet, 
Bull.  Sor.  1906,  (3)  36.  1064.) 

Not  completely  insol.  in  acetic  acid.  (Bau- 
bigny,  Bull.  Soc.  1907,  (4)  1.  58.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Barium  ^chromate,  BaCr2O7+2H2O. 

Decomp.  by  H2O  with  separation  of 
BaCrO4.  Sol.  in  H2CrO4+Aq.  (Bahr,  J.  B. 
1853.  358.) 

Sol.  in  cold  H2O  with  formation  of  BaCrO4 
and  CrO3. 

Insol.  in  glacial  acetic  acid.  (Mayer,  B. 
1903,  36.  1742.) 

Barium  calcium  chromate,  BaCa(CrO4)2. 
(Bourgeois  Bull.  Soc.  Min.  1879,  2.  124.) 

Barium  potassium  chromate,  BaK2(CrO4)2. 

Decomp.  by  H2O.  (Groger,  Z.  anorg. 
1907,  54.  186.) 

Decomp.  by  H2O.  Stable  in  K2CrO4-fAq, 
containing: 

2.181  pts.  K2CrO4  per  100  pts.  H2O  at  11.5° 
3.395  "  "  "  "  "  "  "  27  5° 
5.120  "  "  "  "  "  "  "  50.0° 
7.119  "  "  "  "  "  "  "  76.0° 
9.036  "  "  "  "  "  "  "100.0* 
(Barre,  C.  R.  1914,  158.  497.) 

Barium  potassium  fn'chromate, 

Ba2K2(Cr3Oio)3+3H2O. 
Extremely  deliquescent.    (Bahr.) 

Bismuth  chromates,  basic. 

These  comps.  are  insol.  in  H2O  even  in 
presence  of  H2Cr04;  sol.  in  HC1  or  HNOj-f- 
Aq.  (Lowe,  J.  pr.  67.  288.; 

100  pts.  H2O  dissolve  0.00008  pt.  "bis- 
muth chromate";  100  pts.  acetic  acid  dis- 
solve 0.00021  pt.  "bismuth  chromate";  100 
pts.  HNO3+Aq  (sp.  gr.  =  1.038)  dissolve 
0.00024  pt.  "bismuth  chromate";  100  pts. 
KOH+Aq  (sp.  gr.  =  1.33)  dissolve  0.00016 
pt.  "bismuth  chromate."  (Pearson,  Phil. 
Mag.  (4)  11.  206.) 

Not  insol.  in  dil.  HNO»+Aq  unless  K2CrO4 
is  present.  Less  sol.  in  hot  NaOH+Aq  than 
PbCrO4.  (Storer.) 

"Bismuth  chromate"  is  insol.  in  acetone. 
(Naumann,  B.  1904,  37.  4329.) 

3Bi2O3,  2CrO3  =2(BiO)2CrO4,  Bi2O3.  Insol. 
in  H2O;  sol.  in  HNO3+Aq. 

Bi2O3,  CrO3=  (BiO)2CrO4.  Insol.  in  H2O; 
easily  sol.  in  dil.  HCl+Aq,  less  in  dil.  HNO» 
or  H2SO4+Aq.  (Muir.) 

Bi2O3,  2CrO3  =  (BiO)2Cr2O7.  Insol.  in 
H20. 

+H20. 

5Bi2O3,  HCrO3+6H2O.  .  (Muir,  Chem. 
Soc.  31.  24.) 


254 


CHROMATE,  BISMUTH,  ACID 


3Bi2O3,  7CrO3.  Insol.  in  H2O;  easily  sol.  in 
mineral  acids,  especially  HCl+Aq.  Partly 
sol.  inKOH+Aq. 

Bismuth  chromate,  acid,  Bi2O3,  4CrO3+H2O. 
Insol.  in  hot  or  cold  H2O.    Sol.  in  dil.  HC1 
or  HNOs+Aq.    (Muir,  Chem.  Soc.  30.  17.) 

Bismuth  potassium  chromate,  Bi2(CrO4)3, 
K2CrO4. 

Insol.  in  H2O.    Decomp.  with  hot  H2O. 

Bi2O3,  K2O,  6CrO3+H2O.  (Preis  and  Ray- 
mann,  J.  B.  1880.  336.) 

Bromomolybdenum  chromate. 

(Atterberg.) 

Cadmium  chromate,  basic,  2CdO,  CrO3  + 
H2O. 

Very  si.  sol.  in  H2O;  very  slowly  sol.  in 
NH4OH+Aq  with  combination.  (Malaguti 
and  Sarzeau,  A.  ch.  (3)  9.  431.) 

Composition  as  above.    (Freese,  B.  2.  478.) 

Cadmium  chromate,  CdCrO4. 

Insol.  in  H2O;  sol.  in  acids;  decomp.  by 
heating  with  H2O.  (Schulz,  Z.  anorg.  1895, 
10.  153.) 

Sol.  in  hot  cone.  CdSO4+Aq.  (Briggs, 
Z.  anorg.  1907,  56.  253.) 

+2H2O.  Decomp.  by  boiling  H2O.  (Schulz, 
Z.  anorg.  1895,  10.  153.) 

Cadmium  t/ichromate,  CdO,2CrO3+H2O. 

Easily  sol.  in  H2O  without  decomp; 
hydroscopic.  (Schulz,  Z.  anorg.  1895,  10. 
152.) 

Easily  sol.  in  H2O  but  decomp.  on  evapo- 
ration. (Groger,  Z.  anorg.  1910,  66.  11.) 

Cadmium  /richromate,  CdCr3Oi9+H2O. 
Deliquescent.    (Groger,  Z.  anorg.  1910,  66. 

12.) 

Cadmium    chromate    ammonia.    CdCrO4, 

4NH3+3H2O. 

Efflorescent.  Decomp,  by  H2O.  Sol.  in 
NH4OH+Aq;  insol.  in  alcohol  and  ether. 
(Malaguti  and  Sarzeau.) 

Cadmium  potassium  chromate,  CdKo(CrO4)2 
+2H20. 

Ppt.  Decomp.  by  H2O.  (Groger,  Z.  anorg. 
1907,  64.  189.) 

3CdO,  K20,  3CrO3+3H2O.  ppt.  (Preis 
and  Raymann,  Sitzungsb.  bohms.  Gesell. 
1880.) 

4CdO,  K2O,  4CrO3+3H2O.  Ppt,  Slowly 
decomp.  by  H2O.  (Groger,  M.  1904,  26.  533.') 

Cadmium  potassium  Bichromate, 

CdCr207,K2Cr207+2H20. 
Sol.  in  H2O;  jsl.  hydroscopic.     (Kriiss,  Z. 
anorg.  1895,  8.  454.) 


Cadmium     Bichromate     mercuric     cyanide, 

CdCr2O7,  2Hg(CN)2+7H2O. 
Sol.    in    H2O    without   decomp.      (Kriiss, 
Z.  anorg.  1895,  8.  460.) 

Caesium  chromate,  Cs2CrO4. 
(Chabrie,  C.  R.  1901,  132.  680.) 
Aq.   solution  sat.   at   30°   contains  47%. 

(Schreinemakers,  C.  C.  1909,  I.  11.) 

Caesium    bichromate,   Cs2Cr2O7. 
(Chabrie,  C.  R.  1901,  132.  680.) 
Much  more  sol.  in  hot  H2O,  than  in  cold. 

(Fraprie,  Am.  J.  Sci.  1906,  (4)  21.  309.) 
Aq.    solution   sat.    at   30°    contains   5.2°. 

(Schreinemakers,  C.  C.  1909,  1.  11.) 

Caesium  bichromate,  Cs2Cr3Oi0. 

Decomp.  by  H2O.  (Schreinemakers,  Chem. 
Weekbl.  1908,  6.  811.) 

Sol.  in  H2O.  (Fraprie,  Am.  J.  Sci.  1906, 
(4)  21.  315.) 

Caesium  ^rachromate,  Cs2Cr4Oi3. 

Sol.  in  H2O  with  decomp.  (Schreine- 
makers, Chem.  Weekbl.  1908,  6.  811.) 

Caesium    cobaltous    chromate, 

CsoCo(CrO4)2+6H2O. 
(Briggs,  Z.  anorg.  1907,  66.  248.) 

Caesium  magnesium  chromate, 

Cs2Mg(CrO4)i>+6H2O. 
(Briggs,  Chem.  Soc.  1904,  85,  680.) 

Caesium    nickel    chromate,    Cs2Ni(CrO4)2 

+6H20. 

Sol.  in  cold  H2O  without  much  change,  but 
decomp.  by  warm  H2O.  (Briggs,  Chem. 
Soc.  1904,  86.  679.) 

Calcium  chromate  basic,  Ca2CrO5+3H2O. 

Sol.  in  230  pts.  H2O  without  decomp. 
(Mylius  and  Wrochem,  Gm.  K.  3.  I,  1385.) 

Calcium  chromate,  CaCrO4. 

Anhydrous.  Very  si.  sol.  in  H2O.  (Sie- 
wert,  J.  B.  1862.  148.) 

Aq.  solution,  sat.  at  18°  contains  2.3% 
CaCrO4;  sp.  gr.  =  1.023.  (Mylius  and 
Wrochem,  B.  1900,  33.  3688.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

+  ^iH2O.  Aq.  solution  sat.  at  18°  con- 
tains 4.4%  CaCrO4;  sp.  gr.  =  1.044.  (Mylius 
and  Wrochem,  B.  1900,  33.  3688.) 

+H2O.    Solubility  in  H2O  at  t°. 
tc  0°          8°         13°       18°      25° 

%  CaCrO4     11.5       10.8       10.3       9.6       9.1 

t°  40°        60°        75°       90°     100° 

%  CaCrO4      7.8        5.7        4.6      3.6       3.1 
(Mylius  and  Wrochem,  Gm.-K.  3.  I,  1386.) 


CHROMATE,  CHROMOUS  POTASSIUM 


255 


Sp.  gr.  of  solution  containing  9.6%  by 
wt.  CaCrO4  at  18°  =  1.096.  (Mylius  and 
Wrochom,  B.  1900,  33,  3688.) 

+2H2O.  Sol.  in  241.3  pts.  H2O  at  14°. 
(Siewert.) 

Sol.  in  34  pts.  H2O.  (Schwarz,  Dingl.  198. 
159.) 

Solubility  of  two  modifications  in  H2O  at  t°. 

•   a  modification. 

t°  0°  20°          30°          45° 

%  CaCrO4       14.75       14.22       13.89       12.53 


/3  modification. 


QC 


18°  19.5°  30°  40° 
%  CaCrO4  9.8  1C  10.3  1G.4  10.4  10.4 
(Mylius  and  Wrochem.  Gm.-K.  3.  I,  1387.) 


a  modification.  Sp.  gr.  of  the  solution  con- 
taining 14.3%  by  wt.  CaCrO4  at  18°  =  1.149. 
(Mylius  and  Wrochem,  B.  1900,  33.  3688.) 

p  modification.  Sp.  gr.  of  the  solution  con- 
taining 10.3%  by  wt.  CaCrO4  at  18°  =  1.105. 
(Mylius  and  Wrochem,  B.  1900,  33.  3688.) 

Easily  sol.  in  H2O  containing  CrO3. 

Insol.  in  absolute  alcohol. 

50  cc.  of  alcohol  (29%)  dissolve  0.608  g. 
CaCrO4;  50  cc.  of  alcohol  (53%)  dissolve  0.44 
g.  CaCrO4.  (Fresenius,  Z.  anal.  30.  672.) 

Sol.  in  acids  and  in  dilute  alcohol.  (Caron 
and  Raquet,  Bull.  Soc.  1906,  (3)  35.  1064.) 

Calcium  Bichromate,  CaCr2O7+3H2O. 
Very  deliquescent.    (Bahr,  J.  pr.  60.  60.) 
In  sat.  solution  at  18°,  61%  CaCr2O7  is 

present.     (Mylius  and  Wrochem,  Gm.-K.  3. 

I,  1387.) 

Sol.  in  acetone.     (Naumann,  B.  1904,  37. 

4328.) 

Calcium    potassium    chromate,    CaCrO4, 
K2Cr04 

(Barre,  C.  R.  1914,  158.  495.) 

+H2O.  Easily  sol.  in  H2O.  (Duncan.) 
Insol.  in  H2O  when  ignited. 

+2H2O.  Easily  sol.  in  H2O,  even  after 
ignition.  Insol.  in  alcohol.  (Duncan,  J.  B. 
1850.  313.) 

Formed  below  45°.  (Barre,  C.  R.  1914, 
158.  495.) 

Sol.  in  cold  H->O.  SI.  sol.  in  sat.  K2CrO4  + 
Aq.  (Groger,  Z.  anorg.  1907,  54.  187.) 

Two  modifications.  Solubility  of  a  modi- 
fication is  somewhat  less  than  that  of  the 
P  modification.  (Wyrouboff,  Bull.  Soc. 
Miri.  1891,  14.  255.) 

Solubility  of  two  modifications  in  H2O  at  t°. 

t°  0°  15° 

Solubility  of  a     23.06        25.06 
a  p     23.01         24.45 

(Rakowski,  C.  C.  1909,  I.  133.) 


4CaCrO4,  K2CrO4. 

5CaCrO4,  K2CrO4.  Sol.  in  much  H2O. 
(Bahr.) 

Calcium  chromate  potassium  sulphate, 
CaCrO4,  K2SO4+H2O. 

Decomp.  by  H2O.  (Hannay,  Chem.  Soc. 
32.  399.) 

CaCrO4,  K2SO4,  K2CrO4.    As  above.    (H.) 

Cerous  chromate. 
Insol.  in  H2O. 

Calcium  strontium  chromate,  CaSr(CrO4)2. 
(Bourgeois,  Bull.  Soc.  Min.  1879,  2.  123.) 

Ceric  bichromate,  CeO2,  2CrO3+2H2O. 

Insol.  in  H2O;  sol.  in  acids;  decomp.  com- 
pletely by  boiling  H2O.  (Bricout,  C.  R. 
1894,  118.  145.) 

Chromic  chromate,  CrO2  =  Cr2O3,  CrO3. 

Insol.  as  such  in  H2O,  but  decomp.  thereby 
into  CrO-j  and  Cr2O3;  decomp.  by  alkaline  and 
many  saline  solutions.  Easily  sol.  in  dil.  acids 
if  recently  pptd,  but  with  difficulty  if  dried  at 
a  high  temp.  (Eliot  and  Storer,  Proc.  Am. 
Acad.  5.  207.) 

Cr5O12  =  Cr2O3,  3CrO3.  Sol.  in  HCl+Aq. 
Very  slowly  sol.  in  HNO3+Aq.  Slowly  de- 
comp. by  H2SO4  or  NH4OH+Aq.  Easily  de- 
comp. by  KOH+Aq. 

Does  not  exist.      (Eliot  and  Storer,  I.e.) 

Cr8O]5  =  3Cr2O3,  2CrO3.  Easily  sol.  in  HC1 
or  HNOs+Aq:  difficulty  sol.  in  acetic  acid. 
Easily  sol.  in  KOH+ Aq.  (Traube,  A.  66. 
108.) 

Existence  doubtful. 

O5O9=2Cr2O3,  CrO3.  Insol.  in  all  acids, 
even  aqua  regia;  slowly  attacked  by  a  boiling 
cone,  solution  of  alkali  hydroxides.  (Geuther 
and  Merz,  A.  118.  62.)  Cr3O5,  according  to 
Wohler. 

Chromic  cupric  chromate,  CuCr4O9,  Cr2O3+ 
12H2O. 

Insol.  in  H2O  and  H2SO4.  Sol.  in  HC1  and 
HNO3.  (Rosenfeld,  B.  1879,  12.  957.) 

6CuO,  Cr2O3,  CrO3+9H2O.  Insol.  in 
H2O.  Sol.  in  acids.  (Rosenfeld,  B.  1879,  12. 
958.) 

Chromic  potassium  chromate,  Cr2H2(CrO4)2, 

K2CrO4(?). 

Insol.  in  H2O,  alcohol,  or  acetic  acid.  Not 
attacked  by  cold  HNO3+Aq;  si.  oxidized 
when  hot.  Insol.  in  cold,  easily  sol.  in  hot 
H2SO4.  SI.  sol.  in  SO2+Aq.  Sol.  in  cone. 
HCl-fAq.  (Tommasi,  Bull.  Soc.  (2)  17.  396.) 

Chromous  potassium  chromate, 

K2CrO4(Cr02)2  =  K2Cr(CrO4)2(?). 
Sat.  cold  solution  in  H2O  contains  9%  of 
the  salt.    Insol.  in  alcohol  and  ether.  (Heintze, 
J.  pr.  (2)  4.  212.) 


256 


CHROMATE,  COBALTOUS,  BASIC 


Cobaltous   chromate,   basic,   3CoO,    CrO3  + 

Ppt.  Decomp.  by  H2O.  (Malaguti  and 
Sarzeau,  A.  ch.  (3)  9.  431.) 

True  formula  is  2CoO,  CrO3+2H2O. 
(Freese,  Pogg.  140.  252.) 

4CoO,  3CrO3+2H2O. 

Decomp.  by  H2O.  (Groger,  Z.  anorg.  1906, 
49.  203.) 

Cobaltous  chromate,  CoCrO4. 

Much  more  sol.  in  H2O  than  NiCrO4. 
Easily  sol.  in  hot  dil.  HNO3+Aq.  (Briggs, 
Z.  anorg.  1909,  63.  327.) 

+2H2O.  Ppt.  (Briggs,  Z.  anorg.  1909, 
63.  328.) 

Cobaltous  ^chromate,  CoCr2O7+H2O. 

Deliquescent.  Very  sol.  in  H2O.  (Briggs. 
Z.  anorg.  1907,  66.  247.) 

Cobaltous  potassium  chromate,  basic. 

K2O,  4CoO,  4CrO3+3H2O. 
Sol.    in   cold   dil.   H2SQ4+Aq.      (Groger, 
Z.  anorg.  1906,  49.  199.) 

Cobaltous  potassium  chromate,  K2Co(CrO4)2 

+2H20. 

Decomp.  by  H2O.  (Groger,  Z.  anorg.  1906, 
49.  200.) 

Cupric  chromate,  basic,  3CuO,  CrO3  + 
2H2O. 

Insol.  in  H20.  Easily  sol.  in  dil.  HNO3-f 
Aq  and  in  NH4OH+Aq.  Decomp.  by  KOH 
+Aq.  (Malaguti  and  fearzeau,  A.  ch.  (3)  9. 
434.) 

7CuO,  2CrO3+5H2O.  Ppt.  (Rosenfeld, 
B.  13.  1469.) 

7CuO,  CrO3+5H20.    Ppt.    (R.) 

Cobaltous     cfo'chromate    mercuric     cyanide, 

CoCr2O7,  2Hg(CN)2+7H2O. 
Very  stable.     Sol.   in   H2O.      (Kriiss,   Z. 
anorg.  1895,  8.  458.) 

Cupric  chromate,  CuCrO4 

Insol.  in  H2O;  very  sol.  in  chromic  acid 
and  in  other  acids;  decomp.  by  boiling  with 
H2O.  (Schulz,  Z.  anorg.  1895,  10.  152.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  827.) 

Cupric  di'chromate,  basic,  CuCr2O7,  2CuO. 
(Stanley,  C.  N.  64.  194.) 

Cupric  ^'chromate,  CuCr2O7+2H2O. 

Deliquescent.  Very  easily  sol.  in  H2O, 
NH4OH+Aq,  and  alcohol.  (Droge,  A.  101. 
39.) 

Aqueous  solution  is  decomp.  by  boiling. 
(Malaguti  and  Sarzeau,  A.  ch.  (3)  9. 456.) 

Very  hygroscopic.  Very  sol.  in  H2O  with- 
out decomp.  (Schulz,  Z.  anorg.  1895,  10. 
150.) 


Cupric  tefrachromate,  CuCr4Oi3+2H2O. 

Deliquescent.  Decomp.  when  its  solution 
in  H2O  is  concentrated.  (Groger,  Z.  anorg. 
1910,  66.  15.) 

Cupric    lead    chromate,    2(PbCrO4,    PbO), 

(2CuCrO4,  CuO). 
Min.  Vauquelinite.    Sol.  in  acids. 

Cupric    potassium    chromate,    basic, 

KCu2(OH)(CrO4)2+H2O. 
Ppt.    (Groger,  M.  1903,  24.  485.) 
3CuO,  K2O,  3CrO3+2H2O.     Nearly  insol. 
in  H2O.    Sol.  in  NH4OH  or  (NH4)2C03+Aq. 
(Knop,  A.  70.  52.) 

Does  not  exist.     (Rosenfeld,  B.  13.  1472.) 
4CuO,   K2O,   4Cr03+H2O.     Decomp.   by 
boiling  H2O.    (Gerhardt.) 

+3H2O.  Decomp.  by  boiling  H2O.  (Gro- 
ger, Dissert.  1880.) 

Cupric     potassium     chromate     ammonia, 

K2Cu(CrO4)2,  2NH3. 

Very  sol.  in  dil.  NH3-f-Aq. ;  decomp.  by  H20. 
(Briggs,  Chem.  Soc.  1904,  85.  672.) 

Cupric  chromate  ammonia,  CuCrO4,  4NH3. 

Decomp.  by  H2O.  Sol.  in  dil.  NH4OH  + 
Aq.  (Parravano  and  Pasta,  Gazz.  ch.  it. 
1907,  37.  (2),  255.) 

4CuCrO4,  3NH3+5H2O.  Sol.  in  HC1  and 
NH4OH+Aq.;  insol.  in  organic  solvents;  easily 
sol.  in  AgNO3+Aq.  (Schuyten,  C.  C.  1900, 
I.  399.) 

2CuCrO4,  7NH3+H2O.  Decomp.  by  H2O. 
Very  sol.  in  dil.  NH4OH+Aq.  (Briggs,  Chem. 
Soc.  1904,  85.  673.) 

3CuO,  2CrO3,  10NH3+2H2O.  Decomp, 
by  H2O;  si.  sol.  or  insol.  in  alcohol,  ether,  or 
NH4OH+Aq.  (Malaguti  and  Sarzeau.) 

Decomp.  by  hot  H2O;  insol.  in  alcohol. 
(Bottger.) 

Cupric     d^chromate     ammonia,     CuCr2O7, 

4NH3+2H20. 

Decomp.  by  H2O.  Sol.  in  dil.  NH4OH  + 
Aq.  (Parravano  and  Pasta,  Gazz.  ch.  it. 
1907,  37.  (2)  255.) 

Cupric    cfo'chromate    mercuric    cyanide, 

CuCr2O7,  Hg(CN)2+5H2O. 
Not  hygroscopic.    Sol.  in  H2O.    (Kriiss,  Z. 
anorg.  1895,  8.  461.) 

Didymium  chromate,  Di2(CrO4)3. 

SI.  sol.  in  H2O,  easily  in  dil.  acids.  (Fre- 
richs  and  Smith,  A.  191.  353.) 

+7H20.    (Cleve.) 

Didymium   potassium   chromate, 

Di2(CrO4)3,  K2CrO4. 
Precipitate.    Decomp.  by  H2O.    (Cleve.) 


CHROMATE,  LEAD 


257 


Dysprosium  chromate,  Dy2(CrO4)3 

+10H2O. 

Very  si.  sol.  in  H2O.  1.0002  pt.  is  sol.  in 
100  pts.  H2O  at  25°.  (Jantsch,  B.  1911,  44. 
1276.) 

Glucinum  chromate,  basic,  GlCrO4,  13G1O  + 
23H2O. 

Ppt.  Insol.  in  H2O.  (Creuzberg,  Dingl. 
163.  449.) 

GlCrO4,  6G1(OH2).  Ppt.  Insol.  in  H20. 
(Glassmann,  B.  1907,  40.  2603.) 

Glucinum  chromate,  GlCrO4+H2O. 

Decomp.  by  H2O  with  separation  of  the 
basic  chromate.  (Glassmann,  B.  1907,  40. 
2603.) 

Gold  (auric)  chromate,  Au2(CrO4)3,CrO3. 
Ppt.    (Orloff,  Ch.  Z.  1907,  31.  1182.) 

Indium  chromate. 
Ppt.  (Meyer.) 

Indium  bichromate. 

Very  sol.  in  H2O.    Known  only  in  solution. 

Iron  (ferric)  chromate,  basic. 

Decomp.  by  H20.     (Maus.) 

Fe2O3,  CrO3.  Insol.  in  H2O,  but  decomp. 
thereby,  or  by  saline  solutions;  easily  sol.  in 
acids.  Sol.  in  H2CrO4+Aq.  (Eliot  and 
Storer,  Proc.  Am.  Acad.  6.  216.) 

Iron  (ferric)  bichromate. 

Sol.  in  H2O  and  alcohol.  (Maus,  Pogg.  9. 
132.) 

Iron    (ferric)    potassium    chromate,    basic, 

2CrO3,  6Fe2O3,  3K2O. 

4CrO3,  3Fe2O3,  4K2O. 

10CrO3,  6Fe2O3,  7K2O. 

HCrOa,  3Fe2O3,  4K2O+9H2O. 

9CrO3,  2Fe2O3,  6K2O+6H2O. 

9CrO3,  2Fe2O3,  6K20  +  10H2O. 

lOCrO,,  3Fe2O3,  6K2O+5H2O. 

7CrO3,  2Fe2O3,  2K2O+7H2O. 

4CrO3,  Fe2O3,  K2O+4H2O. 

6Cr03,  2Fe2O3,  3K2O. 

16CrO3,  4Fe2O3,  5K2O+8H2O. 

Above  compounds  are  ppts.,  insol.  in  H2O, 
alcohol  and  ether.  (Lepierre,  C.  R.  1894, 119, 
1215-18.) 

Iron     (ferric)     potassium     chromate, 

Fe2(Cr04)3,  K2CrO4+4H2O. 
Decomp.  by   much  H2O,   cone.   HC1,   or 
NH4OH+Aq.      Not    decomp.    by    alcohol. 
(Hensgen,  B.  12.  130C.) 

Iron    (ferric)    sodium   chromate,   basic, 

5CrO3,  7Fe2O3,  4Na2O. 
Ppt.    (Lepierre,  C.  R.  1894,  119,  1217.) 


Lanthanum  chromate,  La2(CrO4)3. 

SI.  sol.  in  cold,  more  easily  in  hot  H2O; 
easily  sol.  in  acids.  (Frerichs  and  Smith,  A. 
191.  355.) 

+8H2O.    Ppt.    (Cleve.) 

Lanthanum  potassium  chromate. 

(Cleve.) 

Lead  chromate,  basic,  2PbO,  CrO3  (chrome 
red). 

Insol.  in  H2O;  acetic  acid  dissolves  out  % 
the  PbO.  Sol.  in  KOH+Aq.  (Badams, 
Pogg.  3.  221.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

3PbO.  CrO3.     (Hermann,  Pogg.  28.  162.; 

+H2O.  Ppt.  (Strdmholm,  Z.  anorg.  1904, 
38.  443.) 

Min.  Melanochroile,  Phcenicocroite.  Sol. 
in  acids. 

PbO,  PbCrO4.    Ppt.    (S.) 

Lead  chromate,  PbCrO4. 

Insol.  in  H2O.  Pptd.  from  Pb(NO,)2  in 
presence  of  70,000  pts.  H2O.  (Harting.) 

Calculated  from  electrical  conductivity  of 
PbCrO4+Aq,  1  1.  H2O  dissolves  0.2  mg, 
PbCrO4  at  18°.  (Kohlrausch  and  Rose,  Z, 
phys.  Ch.  12.  241.) 

1  1.  H2O  dissolves  1.2  X  KH  g.  PbCrO4  at 
25°.  (Hevesy,  Z.  anorg.  1913,  82.  328.) 

Sol.  in  dil.  H2SO4+Aq  (Storer);  si.  sol.  in 
dil.  HNO3+Aq. 

Sol.  in  560  pts.  HNO3+Aq  of  1.12  sp.  gr.; 
in  150  pts.  HNO3+Aq  of  1.225  sp.  gr.;  in 
130  pts.  HNOs+Aq  of  1.265  sp.  gr.;  in  80 
pts.  HNO3+Aq  of  1.395  sp.  gr.  (Storeys 
Diet.) 

Solubility  of  PbCrO4  in  HNO3+Aq.  at  18°. 

(Millimols.  per  1.) 

0.1N         0.2N         0.3N         0.4N 

0.506        0.844         1.13     .     1.44 

(Beck  and  Stegmuller,  Z.c.) 

Easily  decomp.  by  hot  HCl+Aq.  (Frese- 
inus.) 

Solubility  of  PbCrO4  in  HCl+Aq. 
(Millimols.  per  1.) 


t° 

0.1N 

0.2N 

0.3N 

0.4N 

0.5N 

0.6N 

18 
25 
37 

0.186 
0.239 
0.357 

0.393 
0.485 
0.744 

0.654 
0.839 
1.31 

1.07 
1.32 
2.10 

1.56 
4.06 
3.28 

2.25 
2.95 
4.69 

(Beck    and    Stegmuller,    Arb.    K.    Gesund. 
Amt.  1910,  34.  446.) 

Insol.  in  HC2H8O2+Aq. 

Easily  sol.  in  KOH,  or  NaOH+Aq.  1  1. 
KOH+Aq  (YZ  normal)  dissolves  11.9  g. 
PbCrO4  at  15°  ;16.2  g.  at  60°;  26.1  g.  at  80°; 


258 


CHROMATE,  LEAD 


38.5  g.  at  102.     (Lachaud  and  Lepierre,  Bull. 

Soc.  (3)  6.  230.) 

Insol.  in  NH4Cl+Aq.     (Brett,  1837.) 
Sol.  in  K2Cr2O7+Aq;  almost  completely 

insol.  in  NH4C2H302,  or  NH4NO3+Aq. 
Not  pptd.  in  presence  of  Na  citrate.    (Spil- 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
'J.  1898,  20.  828.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329.) 

Min.  Crocoite.  Sol.  in  hot  HCl+Aq;  diffi- 
cultly sol.  in  HNO3+Aq;  sol.  in  KOH+Aq. 

Lead  bichromate,  PbCr2O7. 

Decomp.  by  H2O. 

+2H2O.  As  above.  (Preis  and  Raymann, 
B.  13.  340.) 

Lead  lithium  chromate,  PbCrO4,  Li2CrO4. 
(Lachaud  and  Lepierre,  C.  R.  110.  1035.) 

Lead  potassium  chromate,  PbCrO4,  K2Cr04. 

Insol.  in  hot  or  cold  H2O  or  in  alcohol.  Dil. 
acids  dissolve  out  K2CrO4.  (Lachaud  and 
Lepierre,  C.  R.  110.  1035.) 

Decomp.  by  H2O.  Stable  in  contact  with 
solutions  containing: 

8.950  pts.  K2CrO4  per  100  pts.  H2O  at    10° 
8.077     "        "          "    "      "      "      '     27.5° 
7*.629     " 
7.150     " 
6.145     " 
4.940 


(Barre,  C.  R.  1914,  168.  497.) 


37.5° 

50.0° 

76.0° 

100.0° 


Lead  sodium  chromate,  PbCrO4,  NaCrO4. 
Sol.  in  H2O(?).     (Lachaud  and  Lepierre.) 
PbCrO4,   2PbO,    Na2CrO4.      (L.    and   L.) 

Lithium  chromate,  Li2CrO4. 

100  cc.  of  solution  sat.  at  18°  contain  85  g. 
anhydrous  salt.  (Kohlrausch,  B.  A.  B. 
1897.  90.) 

99.94  pts.  are  sol.  in  100  pts.  H2O  at  30°. 
^Schreinemakers,  C.  C.  1905.  II,  1486.) 

+2H2O.  Very  easily  sol.  in  H2O.  (Ram- 
;melsberg,  Pogg.  128.  323.) 

100  g.  H2O  dissolve  111  g.  salt  at  20°. 
(Von  Weimarn,  C.  C.  1911.  II,  1300.) 

Sp.  gr.  of  solution  sat.  at  18°  =  1.574,  and 
contains  52.6%  LiCrO4.  (Mylius  and  Wro- 
chem,  B.  1897,  30.  1718.) 

Lithium  bichromate,  Li2Cr2O7. 

130.4  pts.  are  sol.  in  100  pts.  H2O  at  30°. 
(Schreinemakers,  C.  C.  1905.  II,  1486.) 

+2H2O.  Deliquescent.  Sol.  in  H20. 
(Rammelsberg.) 

Lithium    potassium    chromate,    K2CrO4, 
,      Li2Cr04+^H2O. 
Hydroscopic.    (Zehenter,  M.  1897,  18.  54.) 


Magnesium  chromate,  MgCrO4. 

Sol.  in  H2S04,  and  HC1;  insol.  in  HNO3. 
(Dufau,  C.  R.  1896,  123.  888.) 


Sp.  gr.  of  MgCrO4-f-Aq  sat.  at  b°/4°. 
t°  13.6°  14.5°  13.6° 

&MgCrO4        12.31          21.86          27.71 
p.  gr.  1.0886        1.1641         1.2170 

(Slotte,  W.  Ann.  1881,  14.  19.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

+7H2O.    Easily  sol.  in  H2O.    (Vauquelin.) 

100  cm.  of  solution  sat.  at  18°  contain  60  g. 
MgCrO4.  (Kohlrausch,  B.  A.  B.  1897.  90.) 

Sp.  gr.  of  solution  sat.  at  18  =1.422,  and 
contains  42%  MgCrO4.  (Mylius  and  Wro- 
chem,  B.  1897,  30.  1718.) 

+5H2O.  Very  sol.  in  H2O.  (Wyrouboff, 
Bull.  Soc.  Min.  12.  60.) 

Magnesium  bichromate,  Mg2Cr2O7. 

SoL  in  H2O. 

SI.  sol.  in  alcohol.  (Reinitzer,  Zeit.  angew. 
1913,  26.  456.) 

Magnesium  potassium  chromate,  MgCrO4, 
K2CrO4+2H2O. 

100  pts.  H2O  dissolve  28.2  pts.  at  20°;  34.3 
pts.  at  60°.  (Schweitzer.) 

Sol.  in  H2O.  SI.  sol.  in  sat.  K2CrO4+Aq. 
(Groger,  Z.  anorg.  1907,  54.  188.) 

Insol.  in  alcohol. 

+6H2O.  Efflorescent.  (Briggs,  Chem. 
Soc.  1904,  85.  679. 

Magnesium    rubidium    chromate, 

MgRb2(CrO4)2+6H2O. 
(Briggs,  Chem.  Soc.  1904,  85. 679.)  (Barker, 
Chem.  Soc.  1911,  99.  1327.) 

Magnesium  sodium  chromate. 
(Stanley,  C.  N.  54.  194.) 

Manganous  chromate,  2MnO,   CrO3+H2O. 

Ppt.     Sol.  in  dil.  H2SO4,  or  HNO3+Aq. 

(Warrington  and  Reinsch,  Schw.  J.  3.  378.) 

Manganous  potassium  chromate,  MnCrO4, 
K2CrO4+2H2O. 

Decomp.  by  H20.  Sol.  in  dil.  H2SO4. 
(Groger,  Z.  anorg.  1905,  44.  459.) 

2MnCrO4,  K2CrO4+4H2O.  Sol.  in  H2O. 
(Hensgen,  R.  t.  c.  3.  433.) 

Mercurous  chromate,  basic,  4Hg2O,  3CrO3. 
Very  si.  sol.  in  cold,  more  in  boiling  H2O. 
SI.  sol.  in  HNO3+Aq.    Decomp.  by  HC1+ 
Aq.   SI.  sol.  in  NH4Cl+Aq  or  NH4NO3+Aq. 
(Brett.) 

Does  not  exist.    (Richter,  B.  15.  1489.) 
3Hg2O,  CrO3.    Sol.  in  HNO3+Aq.    (Rich- 
ter.) 


CHROMATE  AMMONIA,  NICKEL 


259 


3Hg2O,  2CrOs.  Ppt.  (Fichter,  Z.  anorg. 
1912,  76.  350.) 

Mercurous  chromate,  Hg2CrO4. 

Very  si.  sol.  in  cold,  more  readily  in  hot 
H2O.  SI.  sol.  in  dil.  HNO3+Aq;  sol.  in  cone. 
HNO3;  sol.  in  KCN+Aq;  insol.  in  Hg2(NO3)2 
+Aq.  (Rose,  Pogg.  53.  124.) 

Less  sol.  in  K2CrO4+Aq.  than  in  H2O. 
(Fichter,  Z.  anorg.  1912,  76.  349.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Mercuric  chromate,  basic,  2HgO,  CrO3. 
Sol.  in  HC1,  and  in  HNO3+Aq.    (Geuther.) 
3HgO,  CrO3.     SI.  sol.  in  H2O.     (Millon.) 
The  only  true  compound.    All  others  are 
mixtures  of  HgO  or  HgCrO4  with  this  com- 
pound.    (Cox,  Z.  anorg.  1904,  40.  155.) 

4HgO,  CrO3.  SI.  sol.  in  H2O.  (Millon,  A. 
ch.  (3)  18.  365.) 

7HgO,  2CrO3.    Easily  sol.  in  warm  HNO3, 
when   freshly   precipitated.      Easily   sol.   in 
HCl+Aq.    (Geuther,  A.  106.  247.)  " 
Does  not  exist.    (Freese,  B.  2.  477.) 
5HgO,  CrO3.      Easily    sol.  in    HCl+Aq. 
Very  si.  sol.  in  HNO3+Aq.     Decomp.  by 
H2O   into— 

6HgO,  CrO3.  Insol.  in  H2O.  (Jager  and 
Kriiss,  B.  22.  2049.) 

Mercuric  chromate,  HgCrO4. 

Decomp.  by  H2O  and  acids  into  basic 
salt.  (Geuther.) 

Sol.  in  acids.  Sol.  in  warm  NH4C1,  or 
NH4NO3+Aq.  Sol.  in  Hg(NO3)2,  orHgCl2  + 
Aq. 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329.) 

Mercuric  bichromate,  HgCr2O7. 
Ppt.    (Gawalowski,  C.  C.  1906.  II,  1307.) 

Mercurous  potassium   chromate, 

Hg2K2(Cr04)2. 

Ppt.:  decomp.  by  H2O.  (Groger,  Z.  anorg. 
1907,54.191.) 

Mercuric  chromate,  basic,  ammonia,  12HgO, 

3CrO3,  2NH3+3H2O. 
(Groger,  Z.  anorg.  1908,  58.  420.) 

Mercuric      chromate     ammonia,      HgCrO4, 

2NH3+H2O. 
(Groger,  Z.  anorg.  1908,  58.  419.) 

Mercuric  chromate  sulphide,  2HgCrO4,  HgS. 
Not  attacked  by  weak  acids.    (Palm,  C.  C. 
1863.  121.) 

Nickel  chromate,  basic,  4NiO,  CrO3+6H2O. 
Insol.  in  H20;  easily  sol.  in  NH4OH+Aq. 
(Malaguti  and  Sarzeau,  A.  ch.  (3)  9.  451.) 


3NiO,  CrO3+6H2O.  Insol.  in  H2O:  sol.  in 
NH4OH+Aq.  (Freese,  J.  B.  1869.  271.) 

2NiO,  CrO3+6H2O.  As  above.  (Schmidt, 
A.  156.  19.) 

5NiO,  2CrO3  +  12H2O.     As  above. 
(Schmidt.) 

Nickel  chromate,  NiCrO4. 

Not  attacked  by  boiling  H2O. 

Nearly  insol.  in  hot  dil.  HNO3.  Slowly  sol. 
in  cone.  HNO3  and  aqua  regia. 

Somewhat  sol.  in  NH3-fAq.  (Briggs,  Z. 
anorg,  1909,  63.  326.) 

Nickel  ^chromate,  2NiCr2O7+3H2O. 

Slowly  sol.  in  cold,  rapidly  sol.  in  hot  H2O. 

Deliquescent.  (Briggs,  Z.  anorg.  1907,  56. 
246.) 

Nickel  potassium  chromate,  NiCrO4,  K2CrO4 
+2H2O. 


(Groger,  Z.  anorg.  1906. 
(Briggs,    Chem. 


Decomp.  by  H2O. 
51.  353.) 

+6H2O.      Efflorescent. 
Soc.  1904,  85.  678.) 

Nickel  rubidium  chromate,  NiRb(CrO4)2  + 

6H2O. 

SI.  efflorescent  at  ord.  temp.  (Briggs, 
Chem.  Soc.  1904,  85.  678.) 

Nickel  chromate  ammonia,  NiCrO4,  6NH3  + 

4H2O. 

Decomp.  by  H2O.  Quite  easily  sol.  in 
NH4OH+Aq  of  0.96  sp.  gr.  (Schmidt.)  In- 
sol. in  alcohol  or  ether. 

Potassium  chromate,  K2CrO4,  K2Cr2O7,  etc. 
System:  K2O,  CrO3,  H2O  at  0° 


100  g.  of  the  sat.  solu- 
tion contain 

Solid  phase 

g.   K2O 

g.  Cr33 

31.18 

26.06 

0'54 

K2Cr04 

19.31 

4.27 

(4 

17.73 

5.50 

(1 

17.06 

11.77 

K 

17.18 

11.91 

u 

17.62 

18.71 

(I 

17.63 

18.72 

tt 

17.61 

18.91 

K2Cr04+K2Cr2O7 

17.79 

19.10 

« 

17.80 

19.10 

n 

10.90 

11.93 

K2Cr2O7 

8.07 

8.93 

> 

1.87 

3.13 

i 

1.41 

3.00 

( 

1.42 

3.01 

t 

0.97 

3.94 

1 

0.78 

22.38 

i 

1.02 

38.83 

i 

1.26 

40.10 

• 

1.36 

40.41 

i 

1.22 

41.70 

(i 

260 


CHROMATE,  POTASSIUM 


System:  K2O,  CrO3,  H20  at  0°—  Continued 

System:  K2O,  CrO3,  H2O  at  30° 

100  g   of  the  sat.  solu- 

100 g.  of  the  sat.  solu- 

tion contain 

Solid  phase 

tion  contain 

Solid  phase 

g.  KsO 

g.  CrOs 

_   *K.(\ 

o     PrOo 

g.  J\2O 

g.  i^/rv/3 

46.8 

26.89 

6i94 

KOH,  2H2O 
K2CrO4 

1.28 

41.75 

K2Cr207 

1.40 

42.10 

tt 

22.25 

3.06 

t( 

1.23 

42.11 

ft 

19.52 

6.99 

it 

1.33 

42.16 

ft 

18.65 

13.72 

(i 

1.31 

42.28 

tt 

18.60 

17.00 

(4 

1.38 

42.48 

tt 

18.70 

17.03 

tt 

1.40 

42.68 

if 

19.12 

20.30 

11 

1.47 

42.93 

K2Cr207+K2Cr3010 

19.35 

21.00 

K2Cr04+K2Cr207 

1.47 

42.95 

u 

15.04 

16.85 

K2Cr207 

1.47 

43.09 

ft 

14.77 

16.51 

« 

1.25 

44.52 

K2Cr3O10 

12.28 

14.57 

N 

1.27 

44.95 

ft 

11.20 

13.11 

t( 

1.18 

45.84 

t( 

4.98 

10.48 

tl 

1.17 

46.84 

tt 

3.07 

19.34 

(( 

1.36 

47.22 

K2CrsO10+K2Cr4013 

2.42 

28.21 

(I 

1.36 

47.31 

( 

2.35 

33.77 

11 

1.40 

47.67 

1 

2.30 

36.78 

(( 

1.24 

48.23 

K2Cr4013 

2.30 

40.41 

(( 

1.35 

51.66 

t 

2.50 

44.50 

K2Cr207+K2Cr3Oio 

1.10 

53.81 

2.25 

49.95 

K2Cr30,o+K2Cr4Oi3 

1.08 

55.63 

t 

1.35 

53.39 

K2Cr4018 

1.16 

56.93 

t 

0.69 

62.81 

K2Cr4013+Cr08 

0.96 

57.63 

t 

. 

62.52 

Cr03 

1  16 

59.46 

i 

0.91 

59.87 

• 

(Koppel  and  Blumenthal,  Z.  anorg.  1907,  53. 

0.81 

60.16 

ft 

235.) 

0.70 

61.76 

K2Cr4018+Cr03 

0.62 

61.77 

ft 

0.57 

61.78 

n 

System:  K2O,  CrO3,  H2O  at  60° 

0  67 

61.86 
61.51 
61.52 

CrO3 

<i 

100  g.  of  the  sat.  solu- 
tion contain 

Solid  phase 

61.55 

tt 

g.  K20 

g.  CrOs 

fil    *V7 

it 

"   "   * 

U  1  .  O  i 

c,  50.0 
32.98 
21.05 

6'.  53 
9.15 

KOH,  H20 

K2CrO4 

ft 

(Koppel  and  Blumenthal,  Z.  anorg.  1907,  53. 
94f?  ^ 

A^O.) 

20.70 

8.99 

11 

20.25 

14.43 

it 

20.32 

16.56 

(C 

System:  K2O,  CrO3,  H2O  at  20° 

20.67 
20.72 

r)(\   ao 

21.94 
22.00 

OQ    AQ 

11 

K/~*\/~\         1     TT"    /"^        /~\ 

100  g.  of  the  sat.  solu- 
tion contain 

Solid  phase 

A\)  .  Do 

20.55 
14.53 

Zo.-iy 
23.74 
20.82 

2LrO4+K2Cr2O7 

K2Cr207 
it 

g.  K2O 

g.  CrO3 

13.36 

20.93 

ii 

10.01 

21  24 

a 

2.21 

42.92 

K2Cr207+K2Cr3010 

10.01 

21^24 

(t 

2.20 

43.28 

tt 

8.39 

26.95 

it 

2.10 

44.02 

K2Cr3010 

7.65 

31.49 

tt 

2.02 

45.28 

7.54 

32  92 

u 

2.01 

46.24 

ii 

6.86 

39.64 

u 

2.00 

48.46 

K2Cr3O10+K2Cr4Oi3 

7.06 

49.84 

K2Cr207+K2Cr8010 

1.94 

48.62 

K2Cr4O13 

6.51 

50.40 

K2Cr,Oio 

1.62 

49.01 

ti 

5.33 

52.70 

M 

0.62 

62.80 

K2Cr4O18+CrO8 

5.49 

52.79 

it 

5.06 

53.42 

ft 

(Koppel  and  Blumenthal,  Z.  anorg.  1907,  53. 
243.) 

5^12 
5.30 

53^58 
53.70 

ft 

ft 

CHROMATE,  POTASSIUM 


261 


System:  I 

[20,  Cr03, 

H2O  at  W°~Conlinued 

100  pts.  H2O  dissolve  at— 

100  g.  of  t± 

e  sat.  solu- 

0°           10°  ,       20°          30° 

tion  c 

ontain 

Solid  phase 

58.90       60.92       62.94       64.96  pts.  K2CrO4, 

g.  K2O 

g.  CrOs 

40°          50°          60°          70° 

5.01 

54.09 

K2Cr3010+K2Cr4Oi3 

66.98       69.00       71.02       73.04  pts.  K2CrO4, 

4.G6 

54.73 

K2Cr4013 

3.29 

54.91 

i 

80°          90°        100° 

2.95 

55.43 

i 

75.06       77.08       79.10                pts.  K2CrO4. 

3.01 

56.41 

( 

2.50 

58.05 

t 

(Alluard,  C.  R.  69.  500.) 

2.31 

58.69 

t 

2.00 

60.69 

i 

2.05 

61.25 

t 

100  pts.  H20  dissolve  at— 

1.70 
1.79 
1.57 

61.27 
61.29 
62.57 

» 
( 

i 

0°        10°      27.37°      42.1° 
61.5     62.1       66.3        70.3  pts.  K2CrO4, 

1.27 

65.77 
65.12 

K2Cr4013+Cr03 
CrO3 

63.6°       93.6°       106.1° 

74.9        79.7          81.8  pts.  K2CrO4. 

(Koppel  and  Blumenthal,  Z.  anorg.  1907.  53. 
240.) 

System:  K2O,  CrO3,  H2O  at  the 
cryohydric  pt. 


Cryohy 
dric  pt 

-11.5 
—30.0 
—39.0 

100  g.  of  the  sblu 
tion  contain 

Solid  phase 

g.  K20 

g.  Cr03 

°     17.18 

1.18 
0.79 

18.11 
42.51 
45.69 

K2CrO4+K2Cr2O7 
K2Cr2O7+K2Cr3Oio 
K2Cr3Oio+K2Cr4Oi3 

(Koppel  and  Blumenthal,  Z.  anorg.  1907,  53. 
263-5.) 

B.-pt.  of  solutions  of  CrO3+K20+Aq. 

R.-pt. 

100  g.  of  the  'solu- 
tion contain 

Solid  phase 

g.  K2O 

g.  CrO 

109° 
105.8 
106.8 
104.8 
114.0 
127.0 

30.01 
23.8 
24.3 
16.4 
16.8 

11.92 
25.3 
30.5 
35.6 
59.2 
71.2 

K2Cr04 

a 

K2CrO4+K2Cr2O7 
K2Cr2O7 
K2Cr207+K2Cr3010 
Cr03 

(NordenskjSld   and   Lindstrom,    Pogg.    136. 
314.) 


100  pts.  K2CrO4+Aq  sat.  at  10-12°  con- 
tain 37.14  pts.  salt.  (v.  Hauer,  J.  pr.  103. 

100  pts.  H2O  at  19.5°  dissolve  62.3  pts. 
K2CrO4,  and  solution  has  sp.  gr.  of  1.3787. 
(Schiff,  A.  109.  326.) 


Sat.  K2CrO4+Aq  contains  at — • 
34°         53°         79° 
39.7       40.3       41.8%K2CrO4. 


96° 
42.6 


120° 
44.0 


157° 

45.4%  K2Cr04. 


(Koppel  and  Blumenthal,  Z.  anorg.  1907,  53. 

255.) 

Potassium  chromate,  K2CrO4. 
Easily  sol.  in  H2O. 

Sol.  in  2  pts.  H2O  at  18.75°.     (Ahl.) 

100  pts.  H2O  at  15°  dissolve  43.857  pts.  K2CrO4T  and 
solution  has  sp.  gr.  of  1.3032.  (Michel  and  Krafft,  A. 
ch.  (3)  41.  478.) 

1  pt.  dissolves  in  2.07  pts.  H2O  at  15.5°. 
(Thomson.) 

1  pt.  dissolves  in  1.75  pts.  H2O  at  17.5°, 
and  in  1.67  pts.  HoO  at  100°.  (Moser.) 


(Etard,  A.  ch.  1894,  (7)  2.  550.) 


100  cc.  sat.    K2CrO4+Aq.    contain  53 
K2CrO4  at  18°.     (Kohlrausch,  B.  A.  B. 
90.) 

100  pts.  H2O  dissolve  64.91  pts.  K2CrO4 
at  30°,  or  100  g.  of  solution  contain  39.36  g. 
K2CrO4.  (Schreinemakers,  Chem.  Weekbl. 
1905, 1.  837.) 

100  g.  H2O  dissolve: 

54.57  g.  K2CrO4  at -11.37°  (cryohydric   pt.) 
57.11  g.      "  0° 

65.13  g.  "  "  30° 
74.60  g.  "  "  60° 
88.80  g.  "  "  105.8°  (b-pt.  of  sat.  sol.) 

(Koppel,  Z.  anorg.  1907,  53.  262.) 


64.62  g.  K2CrO4  are  sol.  in  100  g.  H2O  at 
25°.  (Amadori,  Real.  Att.  Line.  1912,  (5)  21, 
I.  667.) 


262 


CHROMATE,  POTASSIUM 


Sp.  gr.  of  K2CrO4+Aq  at  19.5°. 

Insol.  in  liquid  NH3.     (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

o 

c 

100  g.  sat.  solution  in  glycol  at  15.4°  con- 

o 

^ 

3 

Ej 

o 

tain  1.7  g.  K2OO4.    (de  Coninck,  C.  C.  1905, 

C-, 

bj 

Sp.  gr. 

w 

Sp.  «r. 

M 

Sp.  gr. 

II.  183.) 

^ 

^ 

$$ 

Insol.    in    benzonitrile.       (Naumann,    B. 

1914,  47.  1370.) 

1 

1.0080 

15 

.1287 

28 

1.2592 

Insol.  in  methyl  acetate.     (Naumann,  B. 

2 

1.0161 

16 

.1380 

29 

1.2700 

1909,  42.  3790)  ;  "ethyl  acetate.     (Naumann, 

3 

1  0243 

17 

.1474 

30 

1.2808 

B.  1904,  37.  3601.) 

4 

1  .  0325 

18 

.1570 

31 

1.2921 

Insol.  in  acetone.    (Naumann,  B.  1904,  37. 

5 

1  .  0408 

19 

1667 

32 

1.3035 

4329;  Eidmann,  C.  C.  1899.  II,  1014.) 

6 

1  .  0492 

20 

.1765 

33 

1.3151 

-f4H2O.    Easily  sol.  in  H2O  and  in  NH4OH 

7 

1.0576 

21 

.1864 

34 

1.3268 

+Aq.    (Wesch,  Dissert.  1909.) 

8 

1.0663 

22 

.1964 

35 

1.3386 

Potassium  bichromate,  K2Cr2O7. 

9. 
10 
11 

1.0750 
1.0837 
1.0925 

23 
24 
25 

1  2066 
1.2169 

1  .  2274 

36 
37 

38 

1  .  3505 
1.3625 
1.3746 

Sol.  in  H2O,  with  slight  absorption  of  heat. 
Less  sol.  in  H2O  than  K2CrO4. 

12 

1.1014 

26 

1.2379 

39 

1.3868 

Sol.  in  9.6  pts.  H2O  at  17.3°.      (Thompson.) 

13 

1.1104 

27 

1.2485 

40 

1.3991 

10     "       "      "   18.7°.     (Moser.) 

14 

1.1195 



100  pts.  H2O  at  15°  dissolve  9.126  pts. 

(Kremers,  and  Schiff,  calculated  by  Gerlach, 
Z.  anal.  8.  288.) 

K2CrO4  dissolved  in  2  pts.  H2O  has  sp.  gr., 
1.28;  3  pts.,  1.21;  4  pts.,  1.18;  5  pts.,  1.15; 
6  pts.,  1.12;  7  pts.,  1.11;  8  pts.,  1.10.  (Moser.) 

Sp.  gr.  of  sat.  solution  at  8°  =  1.368.  CAn- 
thon,  1837.) 

Sp.  gr.  of  sat.  K2CrO4+Aq  containing 
24.26%  K2CrO4  =  1.2335  at  18°/4°.  (Slotte, 
W.  Ann.  1881,  14.  18.) 

Sp.  gr.  of  K2CrO4+Aq  at  25°. 


(Michel  and  Krafft,  A.  ch.  (3)  41.  478.) 

100  pts.  H2O  dissolve  pts.  K2O2O7.  A  =  ac- 
cording to  Alluard  (C.  R.  59.  500);  K  = 
according  to  Kremers  (Pogg.  92.  497). 


Concentration  of  K2CrO4+Aq. 

Sp.  gr. 

1-normal 
l/r      " 

1U-     " 

Vs-        " 

1.0935 
1.0475 
1.0241 
1.0121 

(Wagner,  Z.  phys.  Ch.  1890,  6.  36.) 

Sat.  K2CrO4  +  Aq  boils  at  107°.    (Kremers.) 

Sat.  K2CrO4+Aq  boils  at  104.2°  under  718 
mm.  pressure.  (Alluard.) 

Freezing  point  of  sat.  K2CrO4+Aq  = 
-12.5°.  (Riidorff.) 

By  dissolving  K2CrO4  in  2  pts.  H2O,  the 
temp,  is  lowered  10°.  (Moser.) 

100  pts.  sat.  solution  of  K2CrO4  and  K2SO4 
contain  37.14  pts.  of  the  two  salts  at  10-12°. 
(v.  Hauer,  J.  pr.  103.  114.) 

Solubility  of  K2CrO4+K2SO4  in  H2O  at  25°. 
(G.  per  100  g.  H2O.) 


K2CrO4 

K2S04 

K2CrO4 

K2S04 

63.09 
61.39 
58.40 
51.81 
40.93 
27.36 

0.76 
1.17 
1.84 
2.36 
3.33 
4.82 

20.83 
14.65 
7.81 
4.36 
1.94 

5.75 
7.12 
8.98 
10.25 
10.86 

(Amadori,  Real.  Att.  Line.  1912,  (5)  21,  I. 
667.) 

t° 

A 

K 

t° 

A 

K 

0 

4.6 

4.97 

60 

45.0 

50.5 

10 

7.4 

8.5 

70 

56.7 

20 

12.4 

13.1 

80 

68.6 

73.0 

30 

18.4 

90 

81.1 

.  . 

40 

25.9 

29.1 

100 

94  1 

102  00 

50 

35  0 

Solubility    in    H2O    at    high    temperatures. 
100  pts.  H20  dissolve  pts.  K2Cr2O7  at  t°. 

t° 

Pts.  K2Cr2O7 

t 

Pts.  K2Cr2O7 

117 

128  3 

148 

200.6 

129 

153  8 

180 

262  7 

(Tilden  and  Shenstone,  Phil. 

Trans. 

1884.23.) 

Solubility  of  K2Cr2O7  in  H2O  at  t°. 

t0' 

%  K2Cr2Q7 

t 

<fy  K2Cr207 

-1 

41 

92 

42.8 

+1 

4.3 

97 

44.0 

6 

5.6 

104 

48.0 

7 

6.1 

120 

52.0 

12 

7.2 

130 

54.4 

15 

8.5 

150 

60.8 

20 

10.4 

157 

62.8 

29 

14.2 

178 

66.6 

36 

16.6 

215 

76.9 

57 

28.2 

291 

89.7 

61 

30.2 

312 

91.8 

65 

32.0 

360 

97.4 

70 

34.4 

(Etard,  A.  ch.  1894,  (7)  2.  550.) 

CHROMATE,  POTASSIUM  YTTERBIUM,  BASIC 


263 


100  g.  H2O  dissolve  10.1  g.  K2Cr,O7  at 
15.5°.  (Greenish  and  Smith,  Pharm.  J.  1901, 
66.  774.) 

100  pts.  H2O  at  30°  dissolve  18.12  pts. 
K2Cr2O7.  (Schreinemakers,  Chem.  Weekbl. 
1905  1.  837.) 

100  g.  H2O  dissolve: 

4.50  g.  K2Cr2O7  at  -0.63°  (cryohydric  pt.) 
4.64  g.        "        "       0° 
18.13  g.        "        "     30° 
45.44  g.        "        "     60° 
108.2  g.        "        "  104.8°  (b-pt.  of  sat.  sol.) 
(Koppel,  Z.  anorg.  1907,  53.  263.) 

100  c.c.  sat.  solution  contain  11.43  g. 
K2Cr2O7  at  20°.  (Sherrill  and  Eaton,  J.  Am. 
Chem.  Soc.  1907,  29.  1643.) 

100  g.  sat.  K2Cr2O7  contain: 

5.52  g.  K2Cr2O7  at    4.81° 

15.17  "          "  30.10° 

.  17  77  «          u  35  330 

(Le  Blanc  and  Schmandt,  Z.  phys.  Ch.  1911, 
77.  614.) 

100  g.  sat.  K2Cr2O7+Aq.  at  35.03°  contains 
17.72  g.  K2Cr2O7.  (Le  Blanc,  Z.  phys.  Ch. 
1913,  86.  335.) 

KzCr-Oy+Aq  sat.  at  8°  has  sp.  gr.  1.065.  (Anthon, 
1837.) 

Sp.  gr.  of  K2Cr2O7+Aq  at  19.5°. 


%  K2Cr2O7 

Sp.  gr. 

%  KaCraO; 

Sp.  gr. 

1 

1.007 

9 

1.065 

2 

1.015 

10 

1.073 

3 

1.022 

11 

1.080 

4 

1.030 

12 

1.085 

5 

1.037 

13 

1.097 

6 

1.043 

14 

1.102 

7 

1.050 

15 

1.110 

8 

1.056 

(Kremers,  calculated  by  Gerlach,  Z.  anal.  8. 

288.) 

Sp.  gr.  of  K2Cr2O7+Aq  containing  4.71% 
K2Cr2O7  =  1.0325  at  ll°/4°;  containing  6.97% 
K2Cr2O7  =  1.0493  at  10.6°/4°.  (Slotte,  W. 
Ann.  1881,  14.  18.) 

Sat.  K2Cr2O7+Aq  boils  at  104°  (Kremers); 
103.4°.  (Alluard). 

Insol.  in  alcohol. 

SI.  sol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Insol.  in  alcohol.  (Ileinitzer,  Zeit.  angew. 
Ch.  1913,  26.  456.) 

100  g.  sat.  solution  in  s;lycol  contain  6  g. 
K2Cr2O7.  (de  Coninck,  ~Bull.  acad.  roy. 
Belg.  1905,  257.) 

Insol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1370.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 


Insol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899.  II,  1014.) 

Potassium  Znchromate,  K2Cr3Ojo. 

Easily  sol.  in  H2O  and  alcohol.  (Bothe,  J. 
pr.  46.  184.) 

Not   deliquescent;   decomp.   by   H2O   in 
chromic  acid  and  K2Cr2O7.  (Jager  and  Krtiss, : 
B.  22.  2041.) 

Potassium  teirachromate,  K2Cr4Oi3. 

Very  deliquescent,  and  easily  sol.  in  H2O. 
(Schwarz,  Dingl.  186.  31.) 

Not  deliquescent.  Decomp.  by  H2O. 
(Jager  and  Kriiss,  B.  22.  2042.) 

Potassium  samarium  chromate, 

K2Sm2(CrO4)4+6H2O. 

Precipitate.     (Cleve.) 
Insol.   in   ethyl  acetate.      (Naumann,    B. 
1904,  37.  3601.) 

Potassium     sodium     chromate,     3K2CrC>4, 

Na2CrO4. 

Sol.  in  H2O.     (v.  Hauer,  J.  pr.  83.  359.) 
64.2  pts.  are  sol.  in  100  pts.  H2O  at  14°. 

(Zehenter,  M.  1897,  18.  49.) 

Potassium  strontium  chromate,  K2Sr(Cr04)2. 
Ppt.  Decomp.  by  H2O.    (Groger,  Z.  anorg. 
1907,  54.  187.) 

Decomp.  by  H2O.  Stable  in  contact  with 
solutions  containing: 

at  11.5°,  2.914  pts.  K2CrO4  per  100  pts.  H2O. 
at  27.5°,  4.123     " 

at    50°,  5.942     "          "        "    "      "      " 
at    76°,  7.920     " 

at  100°,  9.784     "          "        "    "      "      " 
(Barre,  C.  R,  1914,  158.  496.) 

Potassium    thallium    chromate,    K2CrO4, 
Tl2CrO4. 

(Lachaud  and  Lepierre,  Bull.  Soc.  (3)  6. 
232  ) 

+2H2O.  Rapidly  hydrolyzed  by  H2O  un- 
less a  large  excess  of  the  CrO4  ion  is  present. 

Readily  sol.  in  dil.  mineral  acids. 

Difficulty  sol.  in  K2Cr2O7+Aq.  (Hawley, 
J.  Am.  Chem.  Soc.  1907,  29.  304.). 

Potassium    uranyl    chromate,    K2CrC>4, 
2(UO2)CrO4+6H2O. 

Decomp.  by  boiling  with  H2O.  Sol.  in 
acidified  H2O.  (Formanek,  A.  257.  103.) 

K2CrO4,  (UO2)CrO4+H2O;  2K2CrO4, 
3(U02)Cr6  +7H20:   3K2CrO4,   4(UO2)Cr04 
+7H20;  and  K2CrO4,  3(U02)CiO4+14H2O. 

Precipitates.    (Wiesner,  C.  C.  1882.  777.) 

Potassium   ytterbium   chromate,   basic, 

2KYb(Cr04)2+Yb(OH)3+15^H20. 

Ppt.    (Cleve,  Z.  anorg.  1902,  32.  151.) 


264 


CHROMATE,  POTASSIUM  YTTRIUM 


Potassium  yttrium   chromate,   K2CrO4, 

Y2(Cr04)3+*H20. 
Ppt.    (Cleve.) 

Potassium  zinc  chromate,  basic,  K2O,  5ZnO, 
4CrO3+6H2O,  or  K2O,  4ZnO,  3CrO3 
+3H2O. 

Slightly  sol.  in  cold,  decomp.  by  hot  H2O. 
(Wohler.)  ' 

K2O,  4ZnO,  3CrO3+3H2O.  Insol.  in  cold, 
decomp.  by  hot  H2O.  (Groger,  M.  1904, 
26.  520.) 

Potassium    zinc    chromate,    K2Zn(CrO4)2-f 

2H20. 

Ppt.  Decomp.  by  H20.  (Groger,  Z. 
anorg.  1907,  54.  189.) 

Potassium    bichromate    chloride    mercuric 

chloride,  K2Cr2O7,2KCl,4HgCl2+2H2O. 

Solution  in   H20    sat.  at   20.5°  contains 

6.78%   salt.     Salt  is  much  more  sol.  in  hot 

H2O.     (Stromholm,  Z.  anorg.  1912,  76.  278.) 

Potassium  chromate  iodate. 
See  Chromoiodate,  potassium. 

Potassium   chromate   magnesium   sulphate, 

K2CrO4,  MgSO4+9H2O. 
Sol.  in  H2O.    (Etard,  C.  R.  85.  443.) 

Potassium     chromate    'mercuric     chloride, 

K2CrO4,  2HgCl2. 

Easily  sol.  in  H2O.  Sol.  in  dil.  HCl+Aq. 
(Darby.) 

Potassium  Bichromate  mercuric  chloride, 
K2Cr2O7,  HgCl2. 

Ether  or  absolute  alcohol  dissolves  out 
HgCl2.  (Millon,  A.  ch.  (3)  18.  388.) 

Can  be  crystallized  from  H2O.  (Jager  and 
Kruss,  B.  22.  2046.) 

Potassium  chromate  mercuric  cyanide, 
2K2Cr04,  3Hg(CN)2. 

Easily  sol.  in  H2O. 

+H2O.     (Dexter.) 

Formula  is  K2OrO4,  2Hg(CN)2.  (Clarke 
and  Sterne,  Am.  Ch.  J.  3.  352.) 

Potassium    dichromate    mercuric    cyanide, 

K2Cr207,  Hg(CN)2+2H20. 
Sol.  in  H2O.    (Wyrouboff,  J.  B.  1880.  309.) 

Potassium  chromate  phosphate. 
See    Phosphochromate,    potassium. 

Potassium    chromate    sulphate,    K2CrO4, 

6K2SO,. 
Easily  sol.  in  H2O.    (Boutron-Chalard.) 

Potassium  chromate  tellurate. 
See  Chromotellurate,  potassium. 

Rubidium  chromate,  Rb2CrO4. 

Sol.  in  H2O.    (Piccard,  J.  pr.  86.  455.) 


Solubility  in  H2O  at  t°. 


t° 

%  Rb2Cr04 

.  7 

36.65 

0 

38.27 

10.3 

40.22 

20 

42.42 

30 

44.11 

40 

46.13 

50 

47.44 

60.4 

48.90 

(Schreinemakers  and  Filippo,  Chem.  Weekbl. 
1906,  3.  157.) 

Rubidium  bichromate,  Rb2Cr2O7. 

Sol.  in  H2O.  (Grandeau,  A.  ch.  (3)  67 
227.) 

Very  si.  sol.  in  H2O;  5%  at  10°,  8%  at 
26°,  35%  at  60°.  (Wyrouboff,  Bull.  Soc. 
Min.  1881,  4. 129.) 

100  pts.  H2O  dissolve  10.46  pts.  Rb2Cr2O7 
at  30°.  The  solution  contains  9.47%  salt. 
(Schreinemakers  and  Filippo,  Chem.  Weekbl. 
1906,  3.  157.) 

Two  forms  of  crystals.  Figures  denote  pts. 
salt  per  100  pts.  H2O. 

t°  14°      26°       43° 

Monoclinic  form    4.45     8.00     16.52 

Triclinic  form        4.40    7.91     16.57 

(Wyrouboff,  Bull.  Soc.  1908,  (4)  3.  7.) 

Solubility  of  monoclinic  and  triclinic  forms. 


Pts.  of  salt  in 

Pts.  of  salt  in 

100  pts.  H2O 

100  pts.  H2O 

Temp 

Temp 

Mono- 

Tri- 

Mono- 

Tri- 

clinic 

clinic 

clinic 

clinic 

18° 

5.42 

4.96 

40° 

13.22 

12.90 

24° 

6.94 

6.55 

50° 

18.94 

18.77 

30° 

9.08 

8.70 

60° 

28.1 

27.3 

(Stortenbeker,  C.  C.  1907,  II.  1588.) 

Rubidium     bichromate     chloride     mercuric 
chloride,    Rb2Cr2O7,    2RbCl.    4HgCl2  + 
2H2O. 
Sol.  in  H2O. 

Solution  sat.  at  20.5°  contains  5.35%  salt. 
(Stromholm,  Z.  anorg.  1912,  75.  284.) 

Silver  (argentous)  chromate,  Ag4CrO4. 

Sol.  in  dil.  acids.  (Wohler  and  Rauten- 
berg.) 

Existence  very  doubtful. 

Silver  chromate,  Ag2CrO4. 

Absolutely  insol.  in  H2O.  Sol.  in  acids, 
ammonia,  and  alkali  chromates+Aq.  (War- 
ington,  A.  27.  12.) 

Appreciably  sol.  in  cold,  and  still  more  in 
hotH2O.  (Meineke,  A.  261.  341.) 

100  ccm.  H2O  dissolve  0.064  grain  Ag2Cr04 
at  100°;  100  ccm.  H2O  containing  50  grains 


CHROMATE,  SODIUM,  BASIC 


of  the  following  salts  dissolve  the  given  amts. 
of  Ag2CrO4  at  100°:  NaNO3,  0.064  grain; 
KNOs,  0.192  grain;  NH4NO3,  0.320  grain; 
Mg(NO8)2,  0.256  grain.  (Carpenter,  J.  S.  C. 
I.  5.  286.) 

According  to  electrical  conductivity  of 
Ag2CrO4+Aq,  1  1.  H2O  dissolves  28  mg. 
Ag2CrO4  at  18°.  (Kohlrausch  and  Rose,  Z. 
phys.  Ch.  12.  241.) 

1  1.  H2O  dissolves  25  mg.  Ag2CrO4  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1904,  50.  356.) 

25  mg.  are  contained  in  1  1.  of  sat.  solution 
at  18°.  Solubility  increases  unusually  rapidly 
with  temp.  (Kohlrausch,  Z.  phys.  Ch.  1908, 
64.  168.) 

Sol.  in  26,378  pts.  cold  H2O  and  9116  pts. 
HoO  at  100°.  (Koninck  and  Nihoul,  Zeit. 
angew.  Ch.  1891,  5.  295.) 

1  1.  H2O  dissolves  1.2X10-4  gram,  atoms 
of  silver  at  25°.  (Abegg  and  Cox,  Z.  phys. 
Ch.  1903,  46.  11.) 

1  1.  H2O  dissolves  0.029  g.  Ag2CrO4  at  25°. 
(Schafer,  Z.  anorg.  1905,  45.  310.) 

1  1.  H2O  dissolves  0.0256  g.  Ag2Cr04  at 
18°;  0.0341  g.  at 27°;  0.0534  g.  at  50°.  (Whitby 
Z.  anorg.  1910,  67.  108.) 

Sol.  in  hot  NH4OH+Aq  of  sp.  gr.  0.94 
(15.63%  NH3);  si.  sol.  in  cold  NH4OH-f  Aq 
of  sp.  gr.  0.91  (24.99%  NH3).  (Margosches, 
Z.  anorg.  1904,  41.  73.) 


Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  829.)  , 

1 1. 65%  alcohol  dissolves  0.0129  g.  Ag2CrO4 
at  ord.  temp.  (Guerini,  Dissert.  1912.) 

Insol.  in  H2O  containing  acetic  acid  in 
presence  of  large  excess  of  AgNOj.  (Gooch 
and  Weed,  Am.  J.  Sci.  1908,  (4)  26. 85.) 

Practically  insol.  in  glacial  acetic  acid 
but  somewhat  sol.  in  dil.  acetic  acid.  It  be- 
haves in  a  similar  manner  toward  propionic, 
lactic  and  other  organic  acids.  The  red  modi- 
fication is  more  sol.  than  the  greenish-black. 
(Margosches,  Z.  anorg.  1906,  51.  233.) 

Silver  dzchromate,  Ag2Cr2O7. 

SI.  sol.  in  H2O.  Easily  sol.  in  HNO8,  or 
NH4OH+Aq.  (Warington.) 

Decomp.  by  boiling  with  H2O  into  CrO3 
and  Ag2Cr04.  (Jager  and  Kriiss,  B.  22. 
2050.) 

Decomp.  by  cold  H2O.  (Autenrieth,  B. 
1902,  35.  2061.) 

1  pt.  is  sol.  in  12,000  pts.  H2O  at  15°. 
(Mayer,  B.  1903,  36.  1741.) 

Solubility  in  H2O  at  25°  =  7.3X10-3  atoms 
Ag  per  1.  Decomp.  by  HNO3+Aq  (less  than 
0.06  N)  with  separation  of  Ag2CrO4.  (Sherrill 
and  Russ,  J.  Am.  Chem.  Soc.  1907,  29.  1674.) 

Solubility  of  Ag2CrO7  in  HNO3+Aq  at  25°. 


Solubility  of  Ag2CrO 

4inNH4OH+Aqat25°. 

Mols.  HNOs  per  1. 

Milliat. 

per  1. 

Solid  Phase 

Mols.  NH4OH  per  1. 

Mols.  X  103  Ag2CrO4  per  1. 

Cr 

Ag 

0.01 

2.004 

0 

32.20 

5.390 

Ag2CrO4+ 

0.02 

4.169 

Ag2CrO7 

0.04 

8.595 

0.01 

25.06 

6.131 

" 

0.08 

17.58 

0.02 

20.21 

7.148 

n 

0.04 

13.59 

9.529 

" 

(Sherrill  and  Russ.  J 

.  Am.  Chem.  Soc.  1907, 

0.06 

11.10 

11.10 

Ag2Cr2O7 

29. 

1662.) 

0.08 

11.10 

11.10 

" 

SI.  sol.  in  very  cone.  K2CiO4+Aq.    Prac- 

0.08+0.1AgNO3 

6.624 

« 

tically  insol.  in  AgNO3+Aq.    (Margosches.) 

(Sherrill  and  Russ,  J.  Am 

.  Chem. 

Soc.  1907, 

Solubility  of  Ag2CrO4  in  HNO3+Aq  at  25°' 

29.  1664 

) 

Mols. 

Milliat.  per  1. 

Silver  uranyl  chromate,  2Ag2CrO4,  UO2CrO4. 

HNOs 
per  1. 

Cr 

Ag 

Solid  Phase 

Ppt.    (Formanek,  A.  257.  110.) 

0.01 
0.015 
0.02 

3.157 
3.730 
4.177 

6.315 
8^356 

Ag2CrO4 

Silver  chromate  ammonia,  Ag2CrO4,  4JNJ13. 
Decomp.   by  H2O.     Sol.   in  warm   cone. 
NH4OH+Aq.    (Mitscherlich,  Pogg.  12.  141.) 

0.025 

OfkO 

4.567 

Silver    bichromate    mercuric    cyanide, 

.  Uo 

0.04 

5.803 

11.62 

Ag2Cr207,  Hg(CN)2. 

0  05 

6  380 

Sol.  in  cold  H2O;  very  sol.  in  hot  H2O 

0.06 

6.833 

without  decomp. 

(Kriiss, 

Z.  anorg.  1895,  8. 

0.07 

7.333 

456.) 

o!os 

7^477 
7.260 

14.85 
15.45 

4-Ag2Cr2O7 

Ag2Cr2O7,  2Hg(CN)2.    Scarcely  sol.  in  cold, 
more  readily  in  hot  H2O.    Sol.  in  hot  HNO3  + 

0.10 

5.647 

19.01 

» 

Aq,  separating  on  cooling.     (Darby,  Chem. 

0.13 

4.293 

23.89 

11 

Soc.  1.  24.) 

0.14 

3.948 

25.63 

" 

Sodium  chromate,  basic, 

Na4CrO6-f-13H20. 

(Sherrill  and  Russ.  J 

.  Am.  Chem.  Soc.  1907, 

Sol.  without  decomp.  in 

H2O. 

29. 

1663.) 

Sat.    solution 

at    30° 

contains    41.3% 

266 


CHROMATE,  SODIUM 


Na4CrO5.      (Schreinemakers, 
1906,   55.  93.) 

Deliquescent. 
Solubility  in  H2O  at  t°. 
t°    '                   0° 
%  Na4CrO5               33.87 

t°                   27.7° 
%  Na4Cr05               40.09 

Z.    phys 

10° 
35.58 

35° 
44.09 

Ch. 

20.5° 
38.05 

37° 
45.13 

+6H2O. 
Solubility  in  H2O  at  t°. 

t° 

17.7 
19.2 
21.2 

%  Na2  Cr04 

Mols.  H2O  to 
1  mol.  anhy- 
drous salt 

Mols.  anhy- 
drous salt  to 
100  mols.  H2O 

43.65 
44.12 
44.64 

11.60 
11.40 
11.16 

8.62 
8.77 
8.96 

(Mylius  and  Funk,  Gm.-K.  3.  I,  1379.) 

Na4CrO5+Aq  sat.  at  18°  contains  37.50% 
Na4CrO5,  and  has  sp.  gr.  =  1.446.  (Mylius 
and  Funk,  B.  1900,  33.  3688.) 

Sodium  chromate,  Na2CrO4. 

100  ccm.  of  solution  sat.  at  18°  contain 
54  g.  Na2CrO4.  (Kohlrausch,  B.  A.  B.  1897. 
90.) 

Solubility  in  H2O  at  t°. 


t° 

%  Na2CrO4 

70 
80 
100 

55.15 
55.53 
55.74 

(Mylius  and  Funk,  Gm.-K.  3.  I,  1379.) 

Na2CrO4+Aq  sat.  at  18°  contains  40.10% 
Na2CrO4,  and  has  sp.  gr.  =  1.432.     (Mylius 
and  Funk,  B.  1900,  33.  3686.) 
See  also  +4,  6,  and  10H2O. 
Sp.  gr.  of  Na2CrO4+Aq  at  t°/4°. 
t°  17.4°  17.1° 

%  Na2CrO4  5.76  10.62 

Sp.  gr.  1.0576        1.1125 

(Slotte,  W.  Ann.  1881,  14.  18.) 


20.7° 
14.81 
1.1644 


+4H2O.  Sat.  solution  at  30°  contains 
46.62%  Na2CrO4.  (Schreinemakers,  Z.  phys. 
Ch.  1906,  55.  93.) 

Solubility  in  H2O  at  t°. 


t° 

%Na2CrO4 

t° 

49.5 
54.5 
59.5 
65 

%Na2CrO4 

25.6 
31.5 
36 
40 
45 

46.08 
47.05 
47.98 
48.97 
50.20 

50.93 
52.28 
53.39 
55.23 

(Mylius  and  Funk,  Gm.-K.  3.  I,  1379.) 
Solubility  in  H2O  at  t°. 

t° 

%  Na2  Cr04 

Mols.  H20  to 
1    mol  anhy- 
drous salt 

Mols.  anhy- 
drous salt  to 
100  mols.  H20 

28.9 
29.7 
31.2 

46,47 
46.54 
47.08 

10.37 
10.34 
10.12 

9.64 
9.67 

9.88 

(Salkowski,  B.  1901,  34.  1948.) 

(Salkowski,  B.  1901,  34.  1948.) 

+  10H2O.  Deliquescent.  (Kopp,  A.  42. 
99.)  Easily  sol.  in  H2O.  Melts  in  crystal 
H2O  at  23°.  (Berthelot.) 

Sp.  gr.  of  solution  sat.  at  18°  =  1.409,  and 
contains  38.1  %  Na2CrO4.  (Mylius  and  Funk, 
B.  1897,  30.  1718.) 

Solubility  in  H2O  at  t°. 


t° 

%Na2CrO4 

0 
10 
18.5 
19.5 
21 

24.04 
33.41 
41.65 

44.78 
47.40 

(Mylius  and  Funk,  Gm.-K.  3.  I,  1379.) 

Sp.  gr.  of  solution  at  18°  containing  40.1% 
Na2CrO4  =  1.432.  (Mylius,  B.  1900,  33. 
3688.) 

SI.  sol.  in  alcohol.     (Moser.) 

100  g.  absolute  methyl  alcohol  dissolve 
0.345  g.  Na2CrO4  at  25°.  ^(de  Bruyn,  Z.  phys. 
Ch.  10.  783). 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Sodium  efo'chromate,  Na2Cr2O7. 
More  sol.  in  H2O  than  Na2CrO4. 

Solubility  in  H2O  at  t°. 


93' 

98C 


NazCnOz 


81.19 
81.25 


(Mylius  and  Funk,  Gm.-K.  3.  I,  1380.) 

Sp.  gr.  of  aqueous  solution  containing — 
1         5        10       15       20     25%  Na2Cr2O7, 
1.007  1.035  1.071  1.105  1.141  1.171 

30         35        40        45         50  %  Na2Cr2O7. 
1.208   1.245   1.280   1.313    1.343 

(Stanley,  C.  N.  54.  194.) 

Sp.  gr.  of  sat.  solution  containing  63.92% 
Na2€r2O7  at  18°  =  1.745.  (Mylius  and  Funk, 
B.  1900,  33.  3688.) 

SI.  sol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 


CHROMATE,  THALLOUS 


267 


Sol.  in  acetone.     (Naumann,  B.  1904,  37 
4328.) 

+2H2O.    Deliquescent. 

100  pts.  H2O  dissolve  at— 
0°       15°      30°      80°     100°    139° 
•107.2  109.2  116.6  142.8  162.8  209.7  pts.  salt 

(Stanley,  C.  N.  64.  194.) 
Solubility  in  H2O  at  t° 


0 
17 
34. 
52 

72 
81 


%  Na2Cr2O7 


61.98 
63.82 
67.36 
71.76 
76.90 
79.80 


(Mylius  and  Funk,  Gm.-K.  3.  I,  1380.) 

100  g.  H2O  at  30°  dissolve  197.6  g.  Na2Cr2O: 
or  sat.  solution  at  30°  contains  66.4%, 
Na2Cr2O7.  (Schreinemakers,  Z.  phys.  Ch 
1906,  65.  97.) 

100  ccm.  of  a  solution  of  sodium  dichro- 
mate  in  alcohol  contain  5.133  g.  Na2Cr2O7 
2H2O  at  19.4°.  The  solution  decomp.  rapidly. 
(Reinitzer,  Zeit.  angew.  Ch.  1913,  26.  456.) 

The  composition  of  the  hydrates  formed  by 
Na2Cr2O7  at  different  dilutions  is  calculated 
from  determinations  of  the  lowering  of  the 
fr.=  pt.  produced  by  Na2Cr2O7  and  of  the 
conductivity  and  sp.  gr.  of  Na2Cr2O7+Aq. 
(Jones,  Am.  ch.  J.  1905,  34.  317.) 

Sodium  ^nchromate,  NaCr3Oi0. 

Deliquescent.  Very  sol.  in  H2O.  (Stanley, 
C.  N.  54.  194.) 

-fH2O.  Sat.  solution  at  30°  contains 
80%  Na2Cr3O10.  (Schreinemakers,  Z.  phys. 
Ch.  1906,  55.  94.) 

Solubility  in  H2O  at  t°. 

t°    '  0°         15°        55°        99° 

%Na2Cr.,O10        80.03     80.44    82.68     85.78 
(Mylius  and  Funk,  Gm.-K.  3.  I,  1380.) 

Sp.  gr.  of  sat.  solution  containing  80.6% 
Na2Cr3O10  at  18°  =2.059.  (Mylius  and  Funk, 
B.  1900,  33.  3688.) 

Sodium  tetrachr  ornate,  Na2Cr4Oi3+4H20. 
Solubility  in  H2O  at  t°. 

t°    '  0°  16°  22° 

%Na2Cr4013         72.19          74.19          76.01 
(Mylius  and  Funk,  Gm.-K.  3.  1,  1380.) 

Deliquescent. 

Sat.  solution  at  18°  contains  74.6% 
Na2Cr4O13  and  has  sp.  gr.  =  1.926.  (Mylius 
and  Funk,  B.  1900,  33.  3688.) 


Sodium  uranyl  chromate,  Na2CrO4, 
2(UO2)CrO4+10H2O. 

Easily  sol.  in  H2O.  (Formanek,  A.  257. 
108.) 

100  pts.  of  the  solution  in  H2O  contain 
52.52  pts.  of  the  anhydrous  salt  at  20°.  (Rim- 
bach,  B.  1904,  37.  482.) 

Sodium  chromate  silicate,  Na2O,  Cr203, 
2SiO2+14H2O. 

Not  decomp.  by  HCl-fAq.  (Singer,  Dis- 
sert. 1910.) 

2Na2O,  3Cr2O3,  6SiO2.  Not  decomp.  by 
boiling  cone,  acids  -except  HF.  (Weyberg, 
C.  B.  Miner,  1908.  519.) 

5Na2O,  2Cr2O3,  HSiO2.      (Weyberg.) 

3Na2O,  2Cr2O3,  9.5SiO2.     (Weyberg.) 

Strontium  chromate,  SrCrO4. 

Somewhat  sol.  in  H2O.  Sol.  in  840  pts. 
H2O  (Meschezerski,  Z.  anal.  21.  399);  sol.  in 
831.8  pts.  H2O  at  15°.  (Fresenius,  Z.  anal.  29. 
419.) 

100  cc.  H2O  dissolve  0.4651%  at  10°; 
1%  at  20°;  2.417%  at  50°;  3%  at  100°.-  (Rei- 
chard,  Ch.  Z.  1903,  27.  877.) 

Easily  sol.  in  HC1,  HNO3,  or  H2CrO4+Aq. 

Sol.  in  512  pts.  0.5%  NH4Cl-fAq  at  15°. 

Sol.  in  63.7  pts.  1%  HC2H3O2+Aq  at  15°. 

Sol.  in  348.8  pt.s.  solution  containing  0.75% 
NH4C2H3O2,  4  drops  HC2H3O2,  and  6  drops 
(NH4)2Cr04+Aq.  (Fresenius.) 

100  ccm.  NH4Cl+Aq  sat.  at  bpt.  dissolve 
1  g.  SrCrO4.  (Dumesnil,  A.  ch.  1900,  (7)  20. 
125.) 

50  ccm.  alcohol  (29%)  dissolve  0.0066  g. 
SrCrO4. 

50  ccm.  alcohol  (53%)  dissolve  0.001  g. 
SrCrO4.  (Fresenius,  Z.  anal.  30.  672.) 

Strontium  cfo'chromate,  SrCr2O7. 
Easily  sol.  in  H2O. 

Strontium  fn'chromate,  SrCr3Oi0+3H2O. 

Very  deliquescent,  and  sol.  in  H2O.  (Preis 
and  Raymann,  B.  13.  340.) 

Strontium    chromate    mercuric    hydrogen 
chloride,  SrCrO4,  2HgCl2,  HC1. 

According  to  Stromholm  is  SrCl2,  SrCr207, 
4HgCl2+H2O. 

Recryst.  from  H2O.  (Imbert  and  Belugon, 
Bull.  Soc.,  1897,  (3)  17.  471.) 

2SrCrO4,  6HgCl2,  HC1.  (Imbert  and  Belu- 
gon.) 

Thallous  chromate,  TlCrO4. 

100  pts.  H2O  dissolve  0.03  pt.  at  60°. 
Rupp  and  Zimmer,  Z.  anorg.  1902,  33.  157.) 

Ppt.  Insol.  in  cold  moderately  cone. 
HC2H3O2+Aq,  or  in  very  dil.  HNO3+  Aq, 
and  very  si.  sol.  on  boiling  therewith.  Dil. 
S"H4OH,  and  Na2CO3-f  Aq  have  the  same 
action.  Attacked  by  very  dil.  HCl+Aq. 
•>ol.  in  hot  cone.  HCl+Aq.  Decomp.  by  dil. 
HoSO4+Aq.  (Carstanjen.) 


268 


CHROMATE,  THALLOUS 


1 1.  KOH+Aq  (112  g.  per  1.)  dissolves  about 
3.5  g.  Tl2CrO4  on  boiling,  which  separates  out 
on  cooling. 

Boiling  cone.  KOH+Aq  (31%  KOH)  dis- 
solves 18  g.  Tl2CrO4  per  litre.  (Lepierre  and 
Lachaud,  C.  R.  113.  196.) 

Thallous  bichromate,  Tl2Cr2O7. 

Insol.  in  H2O,  etc.  Has  the  same  proper- 
ties as  Tl2CrO4. 

Thallous  bichromate,  Tl2Cr3Oi0. 

Sol.  in  2814  pts.  H2O  at  15°,  and  438.7  pts. 
at  100°.  (Crookes.) 

Thallic  chromate. 
Ppt. 

Thorium  chromate,  basic,  Th(OH)2CrO4. 

Ppt.;  unstable  in  solution.  (Palmer,  Am, 
Ch.  J.  1895,  17.  278.) 

Thorium  chromate,  Th(CrO4)2+H2O. 

Ppt.  Sol.  in  HC1  and  NH4Cl+Aq.    1  pt.  is 

sol.  in  284  pts.  H2O  at  22°.     (Palmer,  Am. 

Ch.  J.  1895,  17.  375  and  278.) 

+3H2O.    Ppt.    (Haber,  M.  1897,  18.  689.) 
+8H2O.      Insol.    in    H2O.      (Chydenius, 

Pogg.  119.  54.) 

Tin  (stannous)  chromate. 

Ppt.     Sol.  in  dil.  acids.     (Berzelius.) 

Tin  (stannic)  chromate. 

Ppt.    (Leykauf,  J.  pr.  19.  127.) 

Uranyl  chromate,   basic,   UO3,   2(UO2)CrO4 

+8H20. 

Ppt.    (Orloff,  Ch.  Z.  1907,  31.  375.) 
UO3,  (UO2)CrO.,+6H2O.    (Orloff.) 

Uranyl  chromate,  (UO2)CrO4+3H2O. 

1  pt.  is  sol.  in  13.3  pts.  H2O  at  15°;  slowly 
sol.  in  alcohol  to  give  a  solution  which  is  de- 
comp.  on  boiling.  (Orloff,  Ch.  Z.  1907,  31. 
375.) 

+  11H20.  Very  sol.  in  H2O.  (Formanek, 
A.  257.  108.) 

Yttrium  chromate. 

Deliquescent.  Easily  sol.  in  H2O.  (Ber- 
lin.) 

Zinc  chromate,  basic,  4ZnO,   Cr03+3H2O. 

(GrSger,  Z.  anorg.  1911,  70.  135.) 

-f  5H2O.  Insol.  in  H2O;  sol.  in  hot  H2Cr04 
+Aq;  slowly  sol.  in  NH4OH+Aq.  (Ma- 
laguti and  Sarzeau,  A.  ch.  (3)  9.  431.) 

3ZnO,  CrO3+2H2O.    (Groger.) 

2ZnO,  CrO3+H2O.  (Briggs,  Z.  anorg. 
1907,  66.  254.) 

+1^H2O.  Ppt.  Insol.  in  H2O.  Sol. 
in  hot  H2CrO4+Aq.  (Prussen  and  Phil- 
lipona,  A.  149.  92.) 


+  2H2O.    Ppt.    Not  wholly  insol.  in  H2O. 
(Prussen  and  Phillipona.) 
3ZnO,  2CrO3+H2O.    (Groger.) 

Zinc  chromate,  ZnCrO4. 

Insol.  in  H2O;  very  sol.  in  acids;  decoinp. 
by  boiling  with  H2O.  (Schulze,  Z.  anorg. 
1895,  10.  154.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  830.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329.) 

+H2O.    (Groger,  Z.  anorg.  1911,  70.  135.) 

Zinc  dichromate,  ZnCr2O7+3H2O. 

Hygroscopic. 

Very  sol.  in  H2O  and  si.  decomp.  by  boiling. 
(Schulze,  Z.  anorg.  1895,  10.  153.) 

Zinc  ^'chromate,  ZnCr3Oio+3H20. 

Deliquescent;  very  sol.  in  H2O.  (Groger, 
Z.  anorg.  1910,  66.  10.) 

Zinc  chromate  ammonia,  ZnCrO4,  NH3+ 
H20. 

Decomp.  by  H2O.  (Groger,  Z.  anorg. 
1908,  58. 417.) 

ZnCrO4,  4NH3+5H2O.  Decomp.  by  H2O. 
Sol.  in  NH4OH+Aq.  Insol.  in  alcohol  and 
ether.  (Malaguti  and  Sarzeau,  A.  ch.  (3)  9. 
431.) 

+3H2O.  Efflorescent.  Decomp.  by  H2O. 
Easily  sol.  in  dil.  acids  and  NH4OH+Aq. 
(Bieler,  A.  151.  223.) 

2ZnO,  3CrO3,  10NH3+10H2O.  Ppt. 
(Malaguti  and  Sarzeau.) 

Zinc  bichromate  mercuric  cyanide,  ZnCr2O7, 

2Hg(CN)2+7H20. 

Very  sol.  in  H20.  Stable  in  aqueous  solu- 
tion at  100°.  (Kruss,  Z.  anorg.  1895,  8. 
460.) 

Perchromic  acid 
See  Perchromic  acid. 

Chromicomolybdic  acid,   Cr2O3,  12MoO3 

+28H20. 

Slowly  sol.  in  H2O.  (Hall,  J.  Am.  Chem. 
Soc.  1907,  29.  708.) 

Ammonium  chromicomolybdate,  3(NH4)2O, 
Cr2O3,  12MoO3+20H2O. 

Sol.  in  H2O.  (Struve,  J.  pr.  61.  457;  Hall, 
J.  Am.  Chem.  Soc.  1907,  29.  695.) 

+26H2O.     (Marckwald,  Dissert,  1895.) 

Ammonium    barium    chromicomolybdate, 
(NH4)2O,     22BaO,     Cr2O3,     12MoO3  + 
20H2O. 
(Hall,  J.  Am.  Chem.  Soc.  1907,  29.  707.) 


CHROMIUM 


269 


Barium   chromicomolybdate,    4BaO,    Cr2O3, 

12Mo03+15H2O;  4BaO,  Cr2O3,  12Mo03 

+  18H2O;     5BaO,     Cr2O3,      12MoO3+ 

16H2O. 

Ppts.    (Hall,  J.  Am.  Chem.  Soc.  1907,  29. 

705.) 

Lead     chromicomolybdate,     4PbO,     Cr2O3, 

12MoO3+22H2O,  and  +24H2O. 
Ppts.    (Hall,  J.  Am.  Chem.  Soc.  1907,  29. 
706.) 

Mercurous       chromicomolybdate,      8Hg2O, 

Cr2O3,  12MoO3+16H2O. 
Ppt.      (Hall,    J.   Am.    Chem.    Soc.    1907, 
29.  707.) 

Potassium  chromicomolybdate,  K2O,  Cr2O3, 
3MoOs. 

Sol.  in  HCl+Aq  with  evolution  of  Cl. 
(Bradbury,  Z.  anorg.  1894,  7.  46.) 

3K2O,  Cr2O3,  12MoO3+20HoO.  Sol.  in 
38.51  pts.  H2O  at  17°.  (Striive;  Hall.) 

+24H2O.    (Hall.) 

4K2O,  Cr2O3,  12MoO3+15H2O.  (Hall,  J. 
Am.  Chem.  Soc.  1907,  29.  709.) 

7K2O,  2Cr2O3,  24MoO3+32H2O.     (Hall.) 

Silver    chromicomolybdate,    5Ag2O,    Cr2O3 

12MoO3-H7H2O. 
Ppt.    (Hall.) 

Sodium    chromicomolybdate,    3Na2O, 

Cr2O3,   12MoO3+21H2O. 
Efflorescent.   Easily  sol.  in  H2O.    (Strtive. 

Chromic  sulphuric  acid. 

See  Sulphochromic  acid. 

Chromicyanhydric  acid, 

H3Cr(CN)6(?). 
Insol.  in  H2O.    (Kaiser,  A.  Suppl.  3.  163. 

Ammonium  chromicyanide,  (NH4)3Cr(CN)6 

Easily  sol.  in  H2O.     (Kaiser.  A.  Suppl.  3 

163.) 

Cupric  chromicyanide,  Cu3[Cr(CN)6]2. 

Ppt.  Insol.  in  dil.  or  cone,  acids,  except  o 
heating.  Insol.  in  NH4OH,  or  KOH+Aq 
(Kaiser.) 

Lead    chromicyanide,    basic,    3Pb(CN)2, 

2Cr(CN)3,  Pb(OH)2. 

Ppt.  Sol.  in  HNO3,  NaOH+Aq,  or  P 
salts +Aq.  (Kaiser.) 

Potassium   chromicyanide,   K3Cr(CN)6. 
Very  sol.  in  H2O. 
100  pts.  cold  H2O  dissolve  30.9  pts.  sal 
Insol.  in  absolute  alcohol,  but  somewha 

sol.  in  dil.  alcohol. 


Sol.    in    cone.    H2SO4    without    decomp. 
Kaiser,  A.  Suppl.  3.  170.) 

ilver  chromicyanide,  Ag3Cr(CN)6 
Insol.  in  all  solvents,  excepting  KCN+Aq. 

Kaiser.) 

Sol.  in  large  excess  of  HCl+Aq.  SI.  sol. 
n  cold,  easily  sol.  in  hot  cone.  HNO3.    Very 

ol.  in  cone.  H2SO4.     Insol.  in  hot  or  cold 

cetic  acid.    (Cruser,  Dissert.  1896.) 

Chromisulphocyanhydric  acid. 

H3Cr(SCN)6. 
Known  only  in  aqueous  solution. 

Ammonium    chromisulphocyamde, 

(NH4)3Cr(SCN)6+4H2O. 
Easily  sol.  in  H2O.    (Rossler,  A.  141. 185.) 

Barium  chromisulphocyanide,  Ba3[Cr(SCN)6]2 

+16H2O. 
Deliquescent,  and  sol.  in  H2O.     (R.) 

Lead  chromisulphocyamde,  Pb3[Cr(SCN)6]2, 

4PbO2H2+8H2O. 

Insol.  in  H2O,  but  decomp.  thereby  into — 
Pb2[Cr(SCN)5]2,  4PbO2H2+5H2O.     Insol. 

nH20. 

Potassium  chromisulphocyanide,  K6Cr(SCN)6 

+4H20. 
'   Sol.  in  0.72  pt.  H2O,  and  0.94  pt.  alcohol. 

Silver    chromisulphocyanide,    Ag6Cr(SCN)«. 
Insol.  in  H2O  or  cone.  HNOs+Aq.    Insol. 
in  NH4OH+Aq.    Sol.  in  KCN+Aq. 

Sodium  chromisulphocyanide,  Na6Cr(SCN)6 

+7H2O. 
Deliquescent;  sol.  in  H2O. 

Chromium, 

Two  modifications — (o)  Not  attacked  by 
H2O.  Easily  sol.  in  cold  HCl+Aq.  SI.  sol. 
in  dil.  H2SO4+Aq.  (Deville.)  Easily  sol. 
in  a  hot  mixture  of  1  pt  H2SO4  and  20  pts. 
H2O.  (Regnault,  A.  ch.  62.  357.)  Easily 
sol.  in  warm  cone.  H2SO4.  (Gmelin.)  Very 
slowly  sol.  in  hot  HNO3+Aq.  (Vauquelin.) 
Insol.  in  dil.  or  cone.  HNO3+Aq.  (Deville.) 
Very  slowly  (Richter),  not  at  all  (Berzelius) 
sol.  in  hot  aqua  regia.  Easily  sol.  in  HF+Aq. 

(jS)  Insol.  in  all  acids,  even  aqua  regia 
(Fremy);  probably  contains  Si. 

Pure  Cr  is  sol.  in  cone.  H2SO4,  HC1  and  dil. 
HNO3;  sol.  in  HgCl2+Aq. 

Insol.  in  fuming  HNOj  and  aqua  regia. 
(Moissan,  C.  R.  1894.  119,  187.) 

Cr  prepared  by  aluminothermic  method 
is  sol.  in  haloid  acids  to  form  chromic  and 
chromous  salts,  even  in  absence  of  air. 
(Doring,  J.  pr.  1902,  (2)  66.  65;  1906,  (2)  73. 
393.) 

Aluminothermic   Cr    is  active  in  contact 


270 


CHROMIUM  AMMONIA  COMPOUNDS 


with  HC1,  HBr,  HI,  HF,  H2SO4,  H2C204, 
i.  e.,  sol.  in  cold  cone,  or  warm  dil.  acids.  Is 
inactive  in  contact  with  cone.  HN03, 
H2Cr2O4,  HC1O3,  HC1O4,  H3PO4,  KOH, 
citric,  formic,  acetic  and  tartaric  acids. 
Cause  attributed  to  a  different  electric  state. 
(Hittorff,  Z.  phys.  Ch.  1898, 25.  729.) 

Chromium  ammonia  compounds. 
See— 
Bromotetramine     chromium     compounds, 

BrCr(NH3)4X2. 

Bromopurpureochromium  compounds, 

BrCr(NH3)5X2. 

•Chlorotetramine     chromium     compounds, 

ClCr(NH3)4X2. 

Chloropurpureochromium  compounds, 

ClCr(NH3)5X2. 

Diamine  chromium  sulphocyanides, 

Cr(-NH3)2(SCN)4M. 

Erythrochromium  compounds, 

(HO)Cr2(NH3)10X2. 

lodopurpureochromium  compounds, 
ICr(NH3)5X2. 

lodotetramine    chromium    compounds, 

ICr(NH3)4X2. 

Luteochromium  compounds,  Cr(NH3)6X3. 
Rhodochromium  compounds, 
(HO)Cr2(NH3)10X5. 

Rhodosc chromium  compounds, 
(HO)3Cr2(NH3)6X3. 

Roseochromium  compounds, 
Cr(NH3)s(OH2)X4. 

Xanthochromium  compounds, 

(H02)Cr(NH3)5X2. 

Chromium  arsenide,  CrAs. 

Insol.  in  mineral  acids.  (Dieckmann,  Z. 
anorg.  1914,  86.  294.) 

Cr2As3.  Insol.  in  mineral  acids.  (Dieck- 
mann.) 

Chromium  azoimide,  CrN3. 

Pptd.  by  addition  of  alcohol  and  ether. 

Insol.  in  H2O.  (Curtius,  J.  pr.  1900,  (2) 
61.  410.) 

Chromium  boride,  CrB. 

Insol.  in  HC1,  dil.  H2SO4,  HF,  HF+HNO3. 

SI.  sol.  in  HNO3  and  in  aqua  regia.  (Wede- 
kind,  B.  1907,  40.  299.) 

Sol.  in  cold  dil.  or  cone.  HC1,  HF,  and 
H2SO4.  (Jassonneix,  C.  R.  1906,  143.  1151.) 

Cr3B2.  Sol.  in  cone,  or  dil.  HF,  HC1, 
H2SO4;  insol.  in  HNO3  or  alkalis +Aq.  (Jas- 
sonneix.) 

Chromous  bromide,  CrBr2 

Sol.  in  H2O.  Not  deliquescent  in  dry  ah1. 
(Moissan,  C.  R.  92.  1051.) 


Chromic  bromide,  CrBr3. 

Anhydrous.  Insol.  in  H2O,  but  dissolves 
at  once  in  presence  of  the  least  trace  of  CrBr2. 
(Bauck,  A.  111.  382.) 

+6H2O.  Deliquescent.  Very  sol.  in  H2O. 
H2O  dissolves  more  than  2  pts.  crystals  at 
ord.  temp.  Very  sol.  in  alcohol.  Insol.  in 
ether.  (Recoura,  C.  R.  110.  1029.) 

Blue  modification.  Insol.  in  alcohol. 
(Recoura,  C.  R.  110.  1193.) 

Very  hygroscopic.  Easily  sol.  in  alcohol 
and  acetone.  Insol.  in  ether.  (Werner,  A. 
1902,  322.  343.) 

+8H2O.  Sol.inH2O.  (Varenne,  C.  R.  93. 
727.) 

Chromium  molybdenyl  bromide, 
CrMo3O4Br4. 

Apparently  wholly  insol.  in  dil.  acids. 
Sol.  in  hot  cone.  HCl+Aq  with  decomp. 
Insol.  in  M2Cr04+Aq.  (Atterberg.) 

-f-2H2O.  Apparently  wholly  insol.  in 
dil.  acids. 

Sol.  in  hot  cone.  HCl+Aq  with  decomp. 

Insol.  in  M2CrO4+Aq.    (Atterberg.) 

Chromic  rubidium  bromide,  CrBr3,  2RbBr 

+H20. 

Sol.  in  H2O  with  decomp.  (Werner,  A. 
1902,322.345.) 

Chromic  bromide  ammonia. 
See  Bromotetramine  chromium  bromide. 


Chromous  bromide  hydrazine, 

CrBr2,  2N2H4. 

Insol.  in  H2O.  Sol.  in  acids.  Insol.  in 
alcohol,  ether  and  similar  solvents.  (Traube, 
B.  1913,46.  1507.) 

Chromium  carbide,  Cr4C. 

(Moissan,  C.  R.  1894,  119.  187.) 

Cr3C2.    Does  not  decomp.  H2O  at  ordinary 

temp,  or  at  100°;  insol.  in  cone.  HC1,  HNO3 

and  aqua  regia;  sol.  in  dil.  HC1  (slowly) ;  insol. 

in  fused  KOH;  sol.  in  fused  KNO3.    (Moissan, 

Bull.  Soc.  1894,  (3)  117.  1016.) 

Chromium  iron  carbide,  3Fe3C,  2Cr3C2. 

Decomp.  by  H2O;  sol.  in  gaseous  hy- 
dracids;  insol.  in  HNO3  and  aqua  regia.  (Wil- 
liams, C.  R.  1898,  127.  484.) 

Chromium  tungsten  carbide,  CW2,  3Cr3C2. 

Not  attacked  by  acids. 

Slowly  attacked  by  fused  KOH  or  alkali 
carbonates.  Rapidly  decomp.  by  fused 
alkali  nitrates  or  KC1O3.  (Moissan,  C.  R. 
1903,  137.  294.) 

Chromous  chloride,  CrCl2. 

Deliquescent.  Very  sol.  in  H2O  with  evolu- 
tion of  much  heat.  (Moberg,  J.  pr.  29.  175.) 


CHROMIC  CHLORIDE 


271 


Practically  insol.  in  ether.  Moderately 
sol.  in  absolute  alcohol,  methyl  alcohol,  and 
acetaldehyde.  (Rohland,  Z.  anorg.  1899,  21. 
39.) 

+l^HoO.    (Moissan,  A.  ch.  (5)  26.  40.) 

+2H2O.  (Knight  and  Rich,  Chem.  Soc. 
1911,  99.  89.) 

+3H2O.    (Knight  and  Rich.) 

Chromous  hydrogen  chloride,  3CrCl2,  2HC1+ 
13H2O. 

Decomp.  by  H2O.  (Recoura,  C.  R.  100. 
1227.) 

SI.  sol.  in  liquid  NH3.     (Gore,  Am.  Ch.  J. 

1898,  20.  827.) 

Chromic  chloride,  CrCl3. 

Anhydrous. — Peach-blossom-colored  modi- 
fication. Insol.  in  pure  H2O  (Peligot),  but 
by  long  continued  boiling  of  the  finely  divided 
salt  with  H2O,  traces  are  dissolved  with 
decomp.  Not  decomp.  by  boiling  eonc. 
H2SO4,  or  other  acids,  even  aqua  regia. 

Easily  sol.  with  evolution  of  heat  in  H2O 
containing  only  V^ooo  pt.  CrCl2.  (Peligot,  J. 
pr.  36. 150).  Also  sol.  in  presence  of  traces  of 
SnCl2  (5  mg.  SnCl2  cause  1  g.  CrCl3  to  dis- 
solve), FeCl2,  Cu2Cl2,  Na2S2O3,  and  other 
reducing  substances;  chlorides  without  re- 
ducing properties  have  no  effect.  (Pelouze,  A. 
ch.  (3)  14.  251).  TiCl3  and  SO2  have  similar 
solvent  action.  (Ebelmen.  A.  ch.  (3)  20.  390); 
also  Zn+dil.  acids.  (Moberg.) 

Insol.  in  dil.  alkalies +Aq;  very  slowly 
decomp.  by  boiling  cone,  alkalies  or  alkali 
carbonates +Aq.  (Fellenberg,  Pogg.  50.  76.) 

Difficulty  sol.  in  methyl  acetate.  (Nau- 
mann,  B.  1909,  42.  3790.) 

Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.  257.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899. 
II,  1014.) 

Practically  insol.  in  absolute  ethyl  alcohol, 
methyl  alcohol,  acetaldehyde  and  ether. 
(Rohland,  Z.  anorg.  189'9,  21.  39.) 

Yellow.  SI.  sol.  in  benzonitrile.  (Nau- 
mann,  B.  1914,  47.  1369.) 

Violet  modification.  Very  sol.  in  H2O  to 
form  a  green  solution.  (Moberg,  J.  pr.  44. 
325.) 

The  violet  mod.  is  almost  insol.  in  H2O 
but  if  V2o,ooo  pt.  chromous  chloride  is  present, 
it  is  readilv  sol.  (Rohland,  £.  anorg.  1899,  21. 
39.) 

+4H2O.  SI.  deliquescent.  Very  sol.  in 
H2O,  alcohol,  and  ethyl  acetate.  (Godeffroy, 
Bull.  Soc.  (2)  43.  229.) 

-f  6H2O.  Deliquescent.  Sol.  in  H2O,  but 
probably  decomp.  to  CrOCl2. 

Practically  insol.  in  ether.  Moderately 
sol.  in  absolute  ethyl  alcohol,  methyl  alcohol 
and  acetaldehyde.  (Rohland,  Z.  anorg. 

1899,  21.  39.) 

" Monochlorochromic  chloride"  is  sol.  in 
ether  and  fuming  HC1(1:1).  (Bjerrum,  B. 
1906,  39.  1599.) 


Time 

Total  Solu- 
bility in  % 

Composition  of  the 
sat.  solution 

%  violet  salt 

%  green  salt 

^hr. 

58.36 

8.30 

91.70 

^hr. 

12.57 

87.43 

4hrs. 

63.27 

24.80 

75.20 

1  day 

68.50 

37.64 

62.36 

2  days 

40.90 

59.10 

3    " 

68.95 

42.78 

57.22 

11    " 

42.84 

57.16 

13    " 

42.39 

57!  61 

19    " 

68.58 

42.62 

57.38 

Green  modification. 

Solubility  in  H2O  at  25°. 
25  g.  green  CrCl3+6H2O  and  10  g.  H2O. 


(Olie,  Z.  anorg.  1906,  51.  55.) 

Solubility  of  green  CrCl3+6H2O  in  H2O  at 
32°. 

10  g.  CrCl3+6H2O  and  4  g.  H2O. 


Time 

Total 
solubility 
in  % 

Composition  of  the 
dissolved  substance 

Solid 
phase 

%  violet 
salt 

%  green 
salt 

r 

45' 
2h5' 
48h 
*lldys. 

63.69 
66.24 
69.53 
69.33 
70.81 

12.87 
21.43 
34.53 
45.27 
45.27 

87.13 
78.57 
65.47 
54.73 
54.73 

Almost 
all 
dis- 
solved 

*  First  8  days  at  35°. 

(Olie,  Z.  anorg.  1907,  63.  276.) 

Solubility  of  green  CrCl8+6H2O  in  H2O  at 
35°. 

10  g.  CrCl3+6H2O  and  3.3  g.  H2O. 


Composition  of  the 

Time 

Total  solubil- 
ity in  % 

dissolved  substance 

%  violet  salt 

%  green  salt 

8' 

65.85 

16.47 

83.53 

38' 

66.74 

25  02 

74.98 

lh 

66.21 

25.45 

74.55 

2h  10' 

68.90 

31.47 

68.53 

4h 

70.79 

36.28 

63.72 

23h 

71.34 

42.95 

57.05 

72h 

70.79 

42.88 

57.12 

(Olie,  I.  c.) 

If  a  solution  saturated  with  the  green  hexa- 
hydrate  below  32°  is  cooled,  the  decahydrate 
separates  out;  if  the  solution  is  saturated 
above  32°,  both  the  decahydrate  and  hexa- 
hydrate  separate  out  on  cooling.  (Olie,  I.  c.) 


272 


CHROMIC  GLUCINUM  CHLORIDE 


Violet  modification. 

Solubility  in  H2O  at  25°. 

25  g.  violet  CrCl3+6H2O  and  10  ccm.  of  a 
35%  solution  of  green  CrCl3+6H2O. 


Composition  of  the 

Composition    of- 

Total  Solu- 

sat.  solution 

the  dissolved 

Time 

Total 

%  violet  salt 

Time 

solubil'y 

Solid  pha^e 

in  % 

IVe  hr. 

65..  49 

84.05 

15.95 

salt 

%  green 
salt 

5    " 
29    " 

84.47 
78  16 

15.53 
21  84 

7' 

61.35 

8.71 

91.29 

CrCl,+10H2O 

2dys. 
4    " 

70.47 

73.19 
68  71 

26.81 
31  29 

20' 
Ih55' 

62.46 
65.04 

9.90 
25.05 

90.10 
74.95 

Cl 

n 

5    " 
5  dys,  6  hrs. 
6dys. 
8    " 

76.38 
73  26 

60.66 
60.36 
65.10 
65  80 

39.34 
39.64 
34.90 
34  20 

4h  30' 
24h 
28h 
29h 

67.41 
69.44 

67  .'59 

32.90 
42.93 
31.78 
33.65 

67.10 
57.07 
68.22 
66.36 

CrCl3+6H2O  . 
all  dissolved 
CrCl3+10H2O 
CrCl8+6H2O 

10    " 

58  08 

41  92 

48h 

69.42 

42.17 

57.83 

ti 

12    " 

71.14 

41.40 

58.60 

72h 

68.69 

43.80 

56.20 

u 

Green  modification. 

Solubility  of  green  CrCl3+10H2O  in  H2O  at 
29°. 

14.2  g.  CrCl3+10H2O  and  2.5  g.  H2O. 


(Olie,  Z.  anorg.  1906,  51.  57.) 

Solubility  in  H2O  at  25°. 
25  g.  violet  CrCl3+6H2O  and  10  g.  H2O. 


Composition  of  the 

Time 

Total  Solu- 

sat.  solution 

bility  in  % 

%  violet  salt 

%  green  salt 

Ve  hr. 

61.99 

98.47 

1.53 

4»/2  hrs. 

96.70 

3.30 

Idy. 

63  .'88 

91.54 

8.46 

2    ' 

.  .  . 

83.37 

•16.63 

4    ' 

70.68 

69.11 

30.89 

5    ' 

62.20 

37.80 

7    ' 

72!il 

62.72 

37.28 

8    ' 

. 

54.63 

45.37 

12    " 

46.39 

53.61 

13    " 

47.66 

52.34 

26    " 

70^62 

48.55 

51.45 

(Olie,  I.  c.) 


Green  modification.  100  pts. 
H2O  dissolve  130  pts.  salt  at  15°.  Sol.  in  al- 
cohol. (Recoura,  C.  R.  102.  518.) 

Grayish-blue  modification.  Very  sol.  in 
H2O.  (Recoura,  C.  R.  102.  548.) 

•flOHjO.  Very  deliquescent;  melts  in 
crystal  H2O  at  6-7°.  Very  sol.  in  H2O,  alcohol, 
and  ethyl  acetate.  (Godeffroy.) 

Easily  sol.  in  H2O;  can  be  recryst.  from 
H2O.  Sol.  in  alcohol  and  ether.  (Werner.  B. 
1906,  39.  1827.) 


(Olie,  Z.  anorg.  1907,  53.  275.) 

The  composition  of  the  hydrates  formed 
byCrCl3  at  different  dilutions  is  calculated 
from  determinations  of  the  lowering  of  the 
fr.  pt.  produced  by  CrCl3  and  of  the  con- 
ductivity and  sp.  gr.  of  CrCl3+Aq.  (Jones, 
Am.  Ch.  J.  1905,  34.  310.) 

Chromic    glucinum    chloride,    CrCl3,    G1C12 

+H20. 

Sol.  in  H2O  with  decomp.  (Neumann,  A. 
244.  329.) 

Chromic   lithium    chloride,    CrCl3,    2LiCl+ 

Very  hygroscopic. 

Sol.  in  ice  water  but  solution  soon  decomp. 

Easily  sol.  in  alcohol.  (Werner,  B.  1901, 
34.  1603.) 

[Cr(OH2)Cl5]Li2+4H20. 

Very  hygroscopic.  Sol.  in  ice  cold  H2O 
and  in  alcohol.  (Werner,  B.  1901,  34.  1604.) 

Chromic  magnesium  chloride,  CrCl3,  MgCl2 

+H2O. 
Decomp.  by  H2O.    (Neumann.) 

Chromic  phosphoric  chloride,   CrClj,   PC15. 
Decomp.  by  H2O.    (Cronander.) 

Chromium    platinum    chloride. 
See  chloroplatinate,  chromium. 

Chromic    potassium    chloride,    CrCl3,    KCL 
Decomp.  by  H2O. 
CrCl3,  2KC1+H2O.     (Neumann,  A.  244. 

CrCls,  3KC1.  Easily  sol.  in  H2O  with  de- 
comp. (Fremy,  A.  ch.  (3)  12.  361.) 


CHROMIC  HYDROXIDE 


273 


Chromic  rubidium  chloride,  CrCl3,  2RbCl+ 
H2O. 

Decomp.  by  H2O.  (Neumann,  A.  244. 
329.) 

Slowly  sol.  in  cold,  rapidly  sol.  in  hot  H2O 
with  decomp.  (Werner,  B.  1901,  34.  1603.) 

CrCl3, 3RbCl+8H2O.  Unstable.  Decomp. 
by  alcohol.  (Werner,  B.  1906,  39.  1830.) 

Chromic  sodium  chloride,  CrCl3,  NaCl. 
Sol.  in  H2O.    (Berzelius.) 
OC13,   3NaCl.     Sol.  in  H2O.    (Berzelius.) 

Chromic  thallium  chloride,  CrCl3,  3T1C1. 

Sol.  with  decomp.  in  H2O.  (Neumann,  A. 
244.  329.) 

Chromic  chloride  ammonia. 
See  Chlorotetramine  chromium  chloride. 

Chromous    chloride    hydrazine,    CrCl2. 

2N2H4. 

Insol.  in  H2O.  Sol.  in  acids.  Insol.  in 
alcohol,  ether  and  similar  solvents.  (Traube, 
B.  1913,  46.  1506. 

Chromic  chloride  ferric  oxide. 

Fe2O3  is  easily  sol.  in  dil.,  difficultly  sol. 
in  cone.  CrCls+Aq.  (Bechamp.  A,  ch.  (3) 
57.  311.) 

Chromous  fluoride,  CrF2. 

SI.  sol.  in  H2O,  hot  H2SO4  or  dil.  HN03. 

Sol.  in  boiling  HC1.  Insol.  in  alcohol. 
(Poulenc,  C.  R.  1893,  116.  254.) 

Chromic  fluoride,  CrF3. 

Perfectly  sol.  in  H2O.     (Berzelius.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  827.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

+3H20.  Insol.  in  H2O.  (Werner  and 
Costachescu,  B.  1908,  41.  4243.) 

+3^H8O.  Sol.  in  H2O.  (Poulenc,  C.  R. 
1893,  116.  255.) 

+6H2O.  SI.  sol.  in  H2O.  (Werner  and 
Costachescu,  B.  1908,  41.  4242.) 

+9H2O.  Violet  modification.  Very  si.  sol. 
in  H2O.  Insol.  in  alcohol.  Sol.  in  HC1,  and 
KOH+Aq.  (Fabris,  Gazz.  ch.  it.  20.  582.) 

Chromium  Aezafluoride,  CrF6. 

Decomp.  by  H2O  with  evolution  of  heat. 
(Berzelius.) 

Correct  composition  is  CrO2F2.  (Oliveri, 
Gazz.  ch.  it.  16.  218.) 

Chromic   cobaltous   fluoride,   CrF3,   CoF2  + 

7H2O. 

Easily  sol.  in  H2O.  (Petersen,  J.  pr.  (2) 
40.  60.) 


Chromic  cupric  fluoride,  CrCuF6+5H2O. 

Can  be  cryst.  from  HF+Aq.  (Higley,  J. 
Am.  Chem.  Soc.  1904,  26.  630.) 

Chromic  nickel  fluoride,  CrF3,  NiF2+7H2O. 

Somewhat  more  sol.  in  H2O  than  CrF8, 

CoF2+7H2O.     (Petersen,  J.  pr.  (2)  40.  61.) 

Chromic  potassium  fluoride,  CrF3,  3KF. 

Nearly  insol.  in  H2O.  (Christensen,  J. 
pr.  (2)  36.  161.) 

CrF3,  2KF+H2O.  Nearly  insol.  in  H2O. 
Sol.  in  cone.  HCl+Aq.  (Christensen.) 

Chromic  sodium  fluoride,  CrF3,  2NaF+H2O. 
(Wagner,  B.  19. 896.) 

Chromic  thallous  fluoride,  2CrF3,  3T1F. 

Sol.  in  hot  H2O,  less  sol.  in  cold.  SI.  sol. 
in  HF.  (Ephraim,  Z.  anorg.  1909,  61.  242.) 

Chromic  zinc  fluoride,  CrF3,  ZnF2+7H2O. 

Can  be  cryst.  from  HF+Aq.  (Higley,  J. 
Am.  Chem.  Soc.  1904,  26.  630.) 

Colloidal  solution  is  perfectly  clear. 
(Biltz,  B.  1902,  36.  4433.) 

Chromous  hydroxide,  CrO2H2. 

Decomp.  by  H2O,  especially  if  hot.  (Pc- 
ligot,  A.  ch.  (3)  12.  539.) 

Slowly  sol.  in  cold  cone,  acids,  even  aqua 
regia;  almost  insol.  in  dil.  acids.  (Moberg,  J. 
pr.43. 119.) 

Chromic  hydroxide,  Cr2O3,  zH2O,  probablv 
Cr206H6. 

Insol.  in  H20.  Easily  sol.  in  acids.  Easily 
sol.  in  cold  KOH,  or  NaOH+Aq;  much  less 
sol.  in  cold  NH4OH+Aq;  the  presence  of 
NH4C1  has  no  influence  upon  solubility 
in  NH4OH+Aq.  (Fresenius.)  Insol.  in 
NH4OH+Aq  if  it  has  been  thoroughly 
washed. 

Insol.  in  KCN+Aq,  but  si.  sol.  in  KCN  + 
HCN+Aq.  (Rodgers,  1834.) 

Gradually  sol.  in  dil.  FeCl3+Aq;  after  three 
months,  2  mols.  Cr2O6H6  are  dissolved  by  1 
mol.  FeCl3  without  pptn.  of  Fe206HG.  (Be- 
champ, A.  ch.  (3)  67. 296.) 

Alsl  sol.  in  CrCl3+Aq;  in  four  months.  \1A 
mols.  Cr2O6H6  are  dissolved  by  1  mol.  CrCl3. 
(Bechamp.) 

Sol.  in  Cr(NO3)3+Aq,  and  clear  solution 
formed  as  long  as  3  mols.  HNO8  are  present 
for  8  mols.  Cr2O3.  (Ordway,  Sill.  Am.  J.  (2) 
27.  197.) 

Chromic  hydroxide,  pptd.  by  alkalies  is 
easily  sol.  in  excess  of  the  reagent;  after  being 
dried  in  a  vacuum,  however,  it  is  insol.  in 
alkalies.  (Herz,  Z.  anorg.  1901,  28.  344.) 

Freshly  pptd.  it  is  sol.  in  aq.  alkali,  but  it 
is  readily  changed  into  a  modification  which  is 
insol.  (Herz,  Z.  anorg.  1902,  31.  352.) 

The  solubility  of  chromic  hydroxide  in  an 


274 


CHROMOCHROMIC  HYDROXIDE 


aqueous  solution  of  red  chromic  chloride  is 
not  directly  proportional  to  the  concentration 
of  the  latter— a  basic  chloride  is  probably 
formed.  (Fischer,  Z.  anorg.  1904,  40.  43.) 

Not  pptd.  in  presence  of  Na  citrate.  (Spil- 
ler.) 

Insol.  in  amylamine+Aq;  not  pptd.  in 
presence  of  alkali  tartrates,  sugar,  etc. 

Cr2O6H6+4H2O.     Difficultly  sol.  in  acids. 

Cr2O6H6-i-H2O.      Extremely    hygroscopic. 

Exists. in  a  soluble  modification,  obtained 
by  dialysis;  solution  can  be  diluted  with  pure 
H2O,  but  gelatinizes  with  traces  of  salts. 
(Graham,  Roy.  Soc.  Trans.  1861.  183.) 

Cr2O2(OH)2.    Insol.  in  boiling  dil.  HC1  + 

Cr2O(OH)4  (Guignet's  green).  Scarcely 
sol.  in  boiling  HCl+Aq.  (Salvetat,  C.  R. 
48.  295.) 

Guignet  gave  formula  as  2Cr203+3H2O. 


Chromochromic  hydroxide,  Cr3O4,  H2O(?). 

Slightly  attacked  by  acids.     (Peligot,  A. 
ch.  (3)  12.  539.) 


Chromous  iodide,  CrI2. 

Easily  sol.  in  H2O.     (Moissan,  A.  ch.  (5) 
25.  401.) 


Chromic  iodide,  CrI3(?). 

Insol.  in  cold,  sol.  in  hot  H2O,  but  no  sepa- 
ration occurs  on  cooling.  (Berlin.) 

-f9H2O.  Hygroscopic.  Sol.  in  alcohol  and 
acetone.  Insol.  in  CHC13.  (Higley,  J.  Am. 
Chem.  Soc.  1904,  26.  628.) 


Chromous   iodide   hydrazine,   CrI2,   2N2H4 
(Traube,  B.  1913,  46.  1507.) 


Chromium  nitride,  ON. 

Insol.  in  dil.  acids  and  alkalies,  cone 
HNO3,  HC1,  or  HF+Aq,  even  on  heating 
Slowly  sol.  in  hot  aqua  regia  or  cold  H2SO4 
Sol.  in  cold  solutions  of  alkali  hypochlorites 
(Ufer,  A.  112.  281.) 

Insol.  in  HC1,  HNO3  and  aqua  regia 
(Feree,  Bull.  Soc.  1901,  (3)  26.  618.) 

Unacted  upon  by  acids  at  ordinary  temper- 
atures. (Smite,  Chem.  Soc.  1897,  72.  (2)  33.) 

Cr3N2.  Slowly  attacked  by  cone.  HNOC 
and  by  HNO8+HC1.  All  other  reagents  are 
without  action.  (Henderson  and  Galletly,  J 
Soc.  Chem.  Ind.  1908,  27.  387.) 

CrN3.    See  Chromium  azoimide. 


Chromous  oxide,  CrO. 

Insol.  in  HNO3  and  dil.  H2SO4+Aq. 

Sol.  in  HC1.     (Feree,  Bull.  Soc.  1901,  (3 
25.  619.) 


Chromic  oxide,  Cr2O3. 

When  ignited  is  nearly  insol.  in  acids,  but 
tissolves  in  H2SO4  by  long  boiling.  Insol. 
n  liquid  HC1.  (Gore.) 

Insol.  in  acetone.  (Fidmann,  C.  C.  1899. 
I,  1014.) 

Solubility  in  (calcium  sucrate+sugar)4- 
Aq. 

1  1.  solution  containing  418.6  g.  sugar  and 
34.3  g.  CaO  dissolves  1.07  g.  Cr2O3;  1  1.  solu- 
;ion  containing  296.5  g.  sugar  and  24.2  g.  CaO 
dissolves  0.56  g.  Cr2O3;  1  1.  solution  contain- 
ing 174.4  g.  sugar  and  14.1  g.  CaO  dissolves 
0.20  g.  Cr2O3.  (Bodenbender,  J.  B.  1865. 
600.) 

See  also  Chromic  hydroxide. 

+H2O.  The  compound  to  which  Bunsen 
gave  the  formula  Cr5O6.  Insol.  in  acids,  but 
easily  attacked  by  HNO3.  (Feree,  Bull.  Soc. 
1901,  (3)  25.  620.) 


Chromochromic  oxide,  Cr3O4  =  CrO,  Cr2O3. 

Known  only  in  form  of  hydroxide,  which 
see. 

+3H2O.  Stable  in  dry  air.  Decomp.  in 
moist  air.  (Bauge,  C.  R.  1898, 127.  552.) 

Cr4O6,  or  Cr6O6  (?).  Insol.  in  acids  or  in 
aqua  regia.  (Bunsen,  Pogg.  91.  622.) 

Not  obtainable.    (Geuther,  A .  118.  66.) 

Formula  is  Cr2O3+H2O.    (Feree.) 


Chromium  ^noxide,  CrO3. 

Deliquescent,   and  very   sol.   in   H2O,    to 
form  solution  of  H2Cr04  or  H2Cr207. 

Solubility  in  H2O  at  t°. 

t°  0°  15°          50°          99° 

%CrO3  62.08      62.38      64.55      67.39 

(Mylius  and  Funk,  Gm.  K.  3.  1,  1332.) 


Sat.  CrO3+Aq  contains  at: 


0° 
61.54 


20° 
62.52 


60° 
65.12%  CrO3. 


(Koppel  and  Blumenthal,  Z.  anorg.  1907,  53. 
228.) 


The  system  CrO3— H2O  has  been  studied 
at  temp,  from  0°to— 74°.  In  the  limits  of 
concentration  investigated,  from  0  —  71.2% 
CrO3,  no  hydrate  of  CrO3  cryst.  from  the 
aq.  solution.  (Kremann,  M.  1911,  32.  622.) 

Sat.  CrO3+Aq  contains  at: 


82° 
66 


100° 
67.4 


115° 
68.4%  Cr03. 


(Kremann,  M.  1911,  32.  620.) 


CHROMIUM  OXIDE  POTASSIUM  CYANIDE 


275 


Solubility  in  H2O  at0. 

B.-pt.  of  CrO3+Aq  at  ord.  pressure. 

t° 

%  by  \vt.  CrOs 

Solid  phase. 

B.-pt.               G.  CrOs  in  100  g.  of  the  solution. 

-0.9° 

3.6 

Ice 

102°                               10.81 

-1.9 

7.8 

it 

104                                24.08 

-3.7 

11.5 

it 

107                                36.47 

-4.8 

14.1 

tf 

110.5                            45.15 

—  10.95 

24.9 

u 

116                                54.56 

-11.7 

25.2 

a 

120                                61.54 

-18.75 

33.5 

it 

127                               71  .  24  sat.  solution 

OK     OK 

OQ     O 

if 

1  -i>)  .  Ad 

-43.5 

49^1 

(Koppel  and  Blumenthal,  Z.  anorg.  1907,  53. 

-60 

53.3 

u 

254.) 

—  20 

61.7 

CrOo 

0 

62.24 

'-  ~~  o 

Sol.  in  H2SO4;  the  solubility  is  least  when 

+24.8 

62.88 

H 

the  acid  contains  66%  H2SO4  (Schrotter); 

40 

63.50 

u 

84.5%  H2SO4  (Bolley). 

65 

64.83 

« 

Verv  sol.  in  H2SO4  of  1.85  sp.  gr.    SI.  sol. 

90 

68.5 

u 

in  cold  KHSO4+Aq.    (Fritzsche.) 

122 

70.7 

If 

The  statement  that  CrO3  is  insol.  in  acids 

193-196 

100 

tt 

is  incorrect.   2.85  g.  (ignited)  are  sol.  in  HNO3 

to  the  extent  of  2.58  g.    0.81  g.  (ignited)  are 

(Buchner  and  Prins,  Z.  phys.  Ch.  1912,  81. 
114.) 

sol.  in  HNO3  to  the  extent  of  0.77  g.    (Jovit- 
schitsch,  M.  1909,  30.  48.) 
Practically  insol.  in  POC13.     (Walden,  Z. 

anorg.  1910,  68.  312.) 

SI.  sol.  in  liquid  NH3.    (Franklin,  Am.  Ch. 

Sp.  gr.  of  CrO3+Aq  at  t°. 

J.  1898,  20.  827.) 

Sol.  in  alcohol  with  decomp. 

t° 

Sp.  gr. 

%  CrOs 

Sol.  in  anhydrous  ether. 

Sol    in  QiCGtio  3/nlivciri.cl.G      fFrv    J    A.m 

16.0 

1.0606 

8 

.25 

Cheni.  Soc.  1911,  33.  702.)  ' 

18.0 

1.0679 

8 

.79 

Sol.  in  acetone.    (Naumann,  B.  1904,  4328.) 

14.5 

1.0694 

8 

.79 

Sol.  in  benzonitrile.     (Naumann,  B.  1914, 

19.5 

1.0957 

12 

.34 

47,  1369.) 

19.0 

1  .  1569 

19 

.33 

Sol.   in  methyl  acetate.      (Naumann,   B. 

20.9 

1  .  20269 

31 

.83 

1909,  42.  3790.) 

20.1 

1.20264 

31 

.83 

Difficultly  sol.   in  ethyl  acetate.      (Nau- 

12.0 

1.20714 

31 

.83 

mann,  B.  1910,  43.  314.) 

35.0 

1  20940 

32 

.59 

18.6 

1.21914 

32 

.59 

Chromium  oxide,  Cr5O9=2Cr2O3,  CrO3. 

15  2 

1.22106 

32 

.59 

/~i      s\       Of***  (~\        Of^W^ 

9.7 
22.0 
19.2 
22.0 

1.22384 
1.3441 
1.3448 
1.34416 
1.7028 

32 
37 
37 
37 
62 

.59 

.77 
.82 
.82 
.23 

V-/1  8^15  —  Ovyl  2^-'3j    A\^'L\J^» 

CrO2  =  Cr203,  CrO3. 
Cr6Oi2=Cr203,  3CrO3. 
Cr6O15  =  Cr2O3,  4CrO3. 
See  Chromate,  chromium. 

(Zettnow,  Pogg.  143.  474.) 

Sp.  gr.  of  CrO8+Aq  (H2CrO4+Aq).  M  = 
according  to  Mendelejeff  at  15  :  Z  =  ac- 
cording to  Zettnow,  calculated  by  Ger- 
lach(Z.  anal.  27.  300). 


%  CrOs 

M 

Z 

%  CrOs 

M 

Z 

5 

.036 

1.037 

35 

1.324 

1.312 

10 

.076 

1.076 

40 

1.383 

1.373 

15 

:  .119 

1.118 

45 

1.445 

1.440 

20 

.166 

1.162 

50 

1.510 

1.512 

25 

.215 

1.208 

55 

1.579 

1.587 

30 

.268 

1.258 

60 

1.656 

More  sol.  in  ether  than  in  H2O.  Ether 
solution  is  somewhat  more  stable  than  aque- 
ous solution.  (Aschoff,  J.  pr.  81.  401.) 

Formula  is  CrO3,  H2O2.  (Moissan,  C.  R. 
97.  96.) 

Chromium  peroxide  ammonia,  CrO4,  3NH3. 

Sol.  in  H2O  with  partial  decomp. 

SI.  sol.  in  NH4OH+Aq. 

Sol.  with  decomp.  in  20%  acetic  acid. 
(Hofmann,  B.  1905,  38.  3060.) 

Chromium   tetfroxide    potassium    cyanide, 

CrO4,  3KCN. 

Sol.  in  H2O.  Insol.  in  other  ordinary 
solvents.  (Wiedo,  B.  1899,  32,  381.) 


276 


CHROMIC  OXYCHLORIDE 


Chromic  oxy chloride. 

From  Cr2O3.  Sol.  in  H2O  as  long  as  1  mol. 
CrCl3  is  present  for  2l/2  mols.  Cr206H6.  (Ord- 
way,  Sill.  Am.  J.  (2)  27.  197.) 

Cr203,  2CrCl3.  Sol.  in  H2O.  (Kletzinsky, 
Zeit.  Ch.  1866.  277.) 

Cr2O3,  CrCl3  =  CrOCl.  Anhydrous.  Only 
partly  sol.  in  H2O. 

+3H2O.  Very  deliquescent,  and  sol.  in 
H2O.  (Peligot.) 

Cr2O3,  4CrCl3+6H20  =Cr2OCl4+2H2O. 
(Peligot,  J.  pr.  37.  38.) 

+9H2O=Cr2OCl4+3H2O.  Sol.  in  H2O 
(Moberg);  =Cr2(OH)2Cl4+2H20.  (Schiff, 
A.  124.  157.) 

Cr2O3,  7CrCl3  =  Cr3OCl7.  Very  sol.  in  H2O 
with  decomp.  (Besson  and  Fo'urnier,  C.  R. 
1909,  148.  1194.) 

Cr2O3,  8CrCl3+24H2O.  Sol.  in  H2O  (Mo- 
berg)  ;  =  Cr2(OH)Cl6+4H2O.  (Schiff,  I.  c.) 

(CrO2)3Cl2.  (Pascal,  C.  R.  1909,  148. 
1464.) 

Cr6O9Cl4.  Insol.  in  H2O.  (Pascal,  C.  R. 
1909,  148.  1464.) 

From  CrO3. 

See  Chromyl  chloride. 

Chromic  oxychloride  potassium  chloride. 
CrOCl3,  2KC1. 

Decomp.  in  the  air. 

Sol.  in  cone.  HC1  without  decomp.  (Wein- 
land,  B.  1906,  39.  4043.) 

Chromic    oxychloride   ruhidium    chloride. 

CrOCl3,  2RbCl. 
Decomp.  in  the  air. 

Sol.  in  cone.  HC1  without  decomp.  (Wein- 
land,  B.  1906,  39.  4045.) 

Chromium  oxyfluoride,  Cr02F2. 
See  Chromyl  fluoride. 

Chromium  phosphide,  CrP. 

Insol.  in  acids,  but  a  trace  dissolves  in 
aqua  regia.  Insol.  in  HF-f  Aq.  (Berzelius.) 

Not  attacked  by  acids  or  by  aqua  regia. 
(Granger,  C.  N.  1898,  77.  228.) 

Insol.  in  all  acids  except  a  mixture  of  HNO3 
and  HF.  (Maronneau,  C.  R.  1900,  130. 
658.) 

Insol.  in  mineral  acids.  (Dieckmann,  Z. 
anorg.  1914,  86.  295.) 

Insol.  in  aqua  regia.  (Granger,  C.  R. 
1897,  124,  191.) 

Cr2P3.  Insol.  in  mineral  acids.  (Dieck- 
mann, Z.  anorg.  1914,  86.  295.) 

Chromous  selenide,  CrSe. 
(Moissan,  C.  R.  90.  817.) 

Chromic  selenide,  Cr2Se3. 

Insol.  in  H,O.     (Moissan,  C.  R.  90.  817.) 


Chromic  potassium  selenide,   K2Cr2Se4. 

Insol.  in  HC1.  Easily  sol.  in  cone.  HNO3. 
(Milbauer,  Z.  anorg.  1904,  42.  451.) 

Chromium  silicide,  Cr2Si. 

Sol.  in  fused  KNO3;  insol.  in  cold  HC1  and 
aqua  regia. 

Insol.  in  HF+Aq.  (Moissan,  C.  R.  1895, 
121.  625.) 

CrSi2.  Sol.  in  HF.  Insol.  in  HC1  and 
aqua  regia.  (Chalmot,  Am.  Ch.  J.  1897,  19. 
69.) 

Cr3Si2.  Insol.  in  dil.  HC1;  sol.  in  warm 
cone.  HC1  and  in  HF;  insol.  in  HNO3  and 
H2SO4.  (Lebeau,  C.  R.  1903,  136.  1330.) 

Cr3Si.  Sol.  in  HF;  insol.  in  other  acids; 
sol.  in  fused  KOH  and  fused  alkali  nitrates 
and  carbonates.  (Zettel,  C.  R.  1898,  126. 
834.) 

Chromous  sulphide,  CrS. 

Insol.  in  H2O  or  K2S+Aq.    (Peligot.) 

Easily  sol.  in  acids.  (Moissan.  C.  R.  90. 
817.) 

Sol.  in  cold  cone,  acids. 

Sol.  in  molten  alkalies.  (Mourlot,  C.  R. 
1895,  121.  944.) 

Min.  Daubrelite. 

Chromic  sulphide,  Cr2S3. 

Insol.  in  H2O  or  alkali  sulphides  +  Aq.  SI. 
attacked  by  HCl+Aq.  (W.  Muller,  Pogg. 
127.  404.) 

HNO3+Aq  decomposes  or  not  according 
to  method  of  preparation.  Easily  decomp. 
by  aqua  regia. 

Insol.  in  caustic  alkalies +Aq. 

Insol.  in  K2S+Aq.     (Berzelius.) 

Chromochromic     sulphide,     Cr3S4,  =CrS, 

Cr2S3. 

Insol.  in  H2O,  HC1,  or  dil.  H2SO4+Aq. 
Easily  sol.  in  HNO3+Aq.  (Groger,  W.  A.  B. 
81.  (2)  531.) 

Chromic  zinc  sulphide,  Cr2ZnS4. 
(Groger,  W.  A.  B.  1880,  81.  534.) 

Chromicyanhydric  acid. 

Cadmium  chromicyanide,  Cd3[Cr(CN)e]2. 

Readily  sol.  in  an  excess  of  KCN  and  in 
NH4OH+Aq.  Decomp.  by  cone.  HC1, 
HNO3  or  H2SO4.  Slowly  decomp.  by  cold, 
rapidly  by  hot  dil.  HC1,  HNO3,  or  H2SO4. 
Quickly  dissolved  by  aqua  regia.  Decomp. 
by  boiling  with  Na2O2,  by  NaOH+Aq  and 
by  Na2CO3+Aq.  Slowly  decomp.  by  boiling 
acetic  acid.  (Cruser  and  Miller,  J.  Am. 
Chem.  Soc.  1906,  28.  1136.) 

Cobaltous   chromicyanide,    Co3[Cr(CN)6]2. 

Sol.  in  cold,  readily  sol.  in  hot  cone.  HC1 
or  H2SO4.  SI.  sol/ even  in  boiling  cone. 


CHROMOSULPHURIC  ACID 


277 


HN03.  Slowly  sol.  in  cold  dil.  H2SO4,  HC1 
or  HNO3.  Readily  sol.  in  boiling  dil.  HC1  or 
H2SO4.  Decomp.  but  not  entirely  dissolved 
by  aqua  regia.  Readily  sol.  in  an  excess  of 
KCN.  Decomp.  by  NH4OH,  NaOH  or 
Na2CO3+Aq.  Decomp.  by  boiling  with 
Na2O2.  Insol.  in  cold  or  boiling  acetic  acid. 
(Cruser  and  Miller.) 

Cuprous  chromicyanide,  Cu3Cr(CN)6. 

Sol.  in  KCN,  cold  cone,  or  boiling  dil. 
HNO3+Aq.  Slowly  sol.  in  cold  cone.  H2SO4, 
still  more  slowly  sol.  in  dil.  H2SO4  but  rapidly 
sol.  in  hot  dil.  and  cone.  H2SO4.  Readily 
decomp.  by  aqua  regia.  Decomp.  by  dil. 
or  cone.  HC1,  slowly  going  into  solution  in 
the  cold,  but  quickly  on  boiling.  (Cruser 
and  Miller.) 

Cupric  chromicyanide,  Cu3[Cr(CN)6]2. 

Slowly  sol.  in  cold  dil.  HC1,  HNO3  or  H2SO4: 
on  boiling  the  first  two  readily  dissolve  it, 
but  the  H2SO4  dissolves  it  only  slowly.  Sol. 
in  aqua  regia  or  cold  cone.  H2SO4.  Readily 
sol.  in  cold  or  hot  cone.  HC1.  Decomp.  by 
cold,  dissolved  by  boiling  HNO3.  Decomp. 
by  boiling  Na2O  2 + Aq .  Decomp .  by  NH4OH, 
NaOH  or  Na2CO3+Aq.  Readily  sol.  in 
an  excess  of  KCN+Aq.  Insol.  in  cold  acetic 
acid.  (Cruser  and  Miller.) 

Nickel  chromicyanide,  Ni3[Cr(CN)6]2. 

Slowly  sol.  in  cold,  readily  sol.  in  hot  dil. 
HC1,  HN03  or  H2SO4.  Slowly  sol.  in  cold, 
readily  sol.  in  hot  cone.  H2SO4,  HC1  or 
HNO3.  Slowly  decomp.  by  cold,  rapidly 
by  boiling  aqua  regia.  Readily  sol.  in  excess 
of  KCN.  Sol.  in  NH4OH+Aq.  Decomp.  by 
NaOH,  Na2CO3+Aq  or  Na2O2+Aq.  Insol. 
in  cold,  si.  sol.  in  boiling  acetic  acid.  (Cruser 
and  Miller.) 

Potassium     tballous     chromicyanide, 

K2TlCr(CN)6. 
(Fischer  and  Benzian,  Ch.  Z.  1902,  26.  50.) 

Thallous  chromicyanide,  Tl3Cr(CN)6. 

Easily  sol.  in  H2O.  (Fischer  and  Benzian, 
Ch.  Z.  1902,  26.  50.) 

Zinc  chromicyanide,  Zn3[Cr(CN)6]2. 

Insol.  in  H2O.  Sol.  in  excess  of  NH4OH, 
NaOH  and  KCN+Aq.  Decomp.  by  Na2C03 
+Aq.  Sol.  in  cold  dil.  HC1.  Slowly  sol. 
in  dil.  H2SO4  and  in  dil.  HNO3.  By  boiling 
with  dil.  acids  a  clear  solution  is  quickly 
obtained.  (Cruser,  Dissert.  1906.) 

Chromisulphocyanhydric  acid. 


Caesium    chromisulphocyanide, 

Cs3Cr(SCN)6+2H2O. 
Less  sol.  in  H2O  than  K  salt. 
Dissert.  1907.) 


(Osann, 


Lithium    chromisulphocyanide, 

Li3Cr(SCN)6+H2O. 
Extremely  deliquescent.    (Osann.) 

Rubidium  cbromisulphocyanide, 

Rb3Cr(SCN)6+4H2O. 
Appreciably  less  sol.  in  H2O  and  alcohol 
than  the  K  salt.    (Osann.) 

Chromocyandric  acid,  H4Cr(CN)6. 

Decomp.  rapidly  on  air.  Sol.  in  H2O 
(Moissan,  A.  ch.  (6)  4. 144.) 

Potassium  chromocyanide,  K4Cr(CN)6. 

Very  sol.  in  H2O;  100  pts.  H2O  dissolve 

32.33  pts.  at  20°.     Much  more  sol.  in  hot 

H2O.     Insol.  in  alcohol,  ether,  benzene,  or 

chloroform.    (Moissan,  A.  ch.  (6)  4.  136.) 

Above  salt  was  K3Cr(CN)6.    (Christensen.) 

+3H20.    (Christensen,  J.  pr.  (2)  31.  166.) 

Chromoiodic  acid,  CrO3,  HIO3+2H2O. 
Deliquescent.    (Berg,  C.  R.  104. 1514.) 

Ammonium  chromoiodate,  CrO3,  NH4IO3+ 

H2O. 
Moderately  sol.  in  H2O.    (Berg.) 

Lithium  chromoiodate,  CrO3,  LiIO3+H2O. 
Very  sol.  in  H2O.    (Berg.) 

Magnesium  chromoiodate. 
Sol.  inH2O.    (Berg.) 

Potassium  chromoiodate,  CrO3,  KIO8. 

Sol.  in  H2O.    (Berg.) 

+H2O  =  KCrIH2O7.  SI.  decomp.  by  H2O. 
(Blomstrand,  J.  pr.  (2)  40.  331.) 

Silver  chromoiodate,  CrO3,  AgI03. 

SI.  attacked  by  cold,  rapidly  decomp.  by 
hot  H2O.  (Berg,  C.  R.  111.  42.) 

Sodium  chromoiodate,  CrO3,  NaIO3+H2O. 
Very  sol.  in  H2O.    (Berg.) 

Chromosulphocyanhydric  acid. 

Sodium  chromosulphocyanide, 
Na3Cr(SCN)6+10,  or  11H2O. 

Unstable. 

Decomp.  by  H2O.  (Koppel,  Z.  anorg. 
1905,  45.  360.) 

Chromosulphuric  acid,  H2Cr2(SO4)4. 

S.ol.  in  H2O  in  all  proportions,  but  solution 
is  easily  decomp.  on  standing  or  boiling. 
(Recoura,  Bull.  Soc.  (3)  9.  586.) 

H4Cr2(SO4)5.    As  above. 

H6Cr2(SO4)6.    As  above. 


278 


CHROMOSULPHATE,  AMMONIUM 


Ammonium  chromosulphate, 
(NH4)2Cr2(S04)4+5H20. 
Sol.  in  H2O  after  a  few  minutes.    (Recoura.) 

Chromium    potassium    chromosulphate, 

[Cr2(S04)3Ci<)4]K2,[Cr2(S04)3(Cr04)2]K4, 
and   [Cr2(SO4)3(CrO4)3]K6. 

Sol.  in  H2O.  (Recoura,  Bull.  Soc.  1897,  (3) 
17.  934.) 

Potassium    chromosulphate,    K2Cr2(SO4)4+ 

4H2O. 

Sol.  in  H2O  in  a  few  minutes.  (Recoura, 
Bull.  Soc.  (3)  9.  590.) 

Sodium    chromosulphate.    Na2Cr2(SO4)4+ 

10H2O. 
As  K  salt.    (Recoura.) 

Chromotelluric  acid. 

Ammonium  chromotellurate, 

2(NH4)20,  4CrO3,  TeO3. 
Sol.  in  H2O.    (Berg,  C.  R.  1911,  162. 1588.) 

Potassium  chromotellurate, 
2K2O,  4Cr03,  TeO3. 

SI.  sol.  in  cold  H2O  without  decomp. 

Sol.  in  boiling  H2O.  (Berg,  Bull.  Soc. 
1911,  (4)  9.  583.) 

Chromous  acid,  H2Cr2O4=Cr2O3,  H2O. 

Chromic  hydroxide  shows  slightly  acid  prop- 
erties, and  salts  corresponding  to  the  above 
acid  are  known. 

Aluminum     ferrous     magnesium     chromite 
(chrome  iron  ore),  (Fe,  Mg)O, 
(Cr2,  A12)03. 
Insol.  in  H2O  or  acids,  even  a  mixture  of 

H2SO4  and  HF.    (Ebelmen.) 

Barium  chromite,  BaCr20<. 

Insol.  in  H2O.  (Gerber,  Bull.  Soc.  (2)  27. 
436.) 

Barium  ^rachromite,  BaO,  4Cr2O3. 

Undecomp.  by  steam  at  red  heat;  insol. 
in  HC1,  H2SO4,  HNO3;  sol.  in  fused  KOH  + 
KN03;  decomp.  in  the  air.  (Dufau,  C.  R. 
1896, 122. 1126.)  . 

Cadmium  chrcmite,  CdCr2O4. 

Not  attacked  by  acids.  (Viard,  C.  R.  109. 
142.) 

Calcium  chromite,  CaCr2O4. 

Insol.  in  H2O.  (Gerber,  Bull.  Soc.  (2)  27. 
436.) 

Insol.  in  HC1,  HF,  HNO3,  H2SO4;  sol.  in 
gaseous  HC1  and  HF  at  red  heat:  sol.  in 
fused  KOH,  KNO3,  KC1O3,  K2CO3.  (Dufau, 
C.  R.  1895,  121.  690.) 


2CaO,  Cr2O3.  Insol.  in  H2O,  KOH,  or 
NH4OH+Aq;  slowly  decomp.  by  H2CO3, 
or  M2CO3-|-Aq;  insol.  in  sugar  solution. 
(Pelouze,  A.  ch.  (3)  33.  9.) 

4CaO,  Cr2O3.  Attacked  by  H2O.  (Mois- 
san,  C.  R.  1894, 119. 188.) 

Cobaltous  chromite,  CoCr2O4. 

(Elliot,  Dissert,  Gottingen,  1862.) 

Cuprous  chromite,  Gu2O,  Gr2O3. 

Insol.  in  HNO3+Aq(sp.  gr.  1.4).  (Wohler, 
Z.  phys.  Ch.  1908,  62.  445.) 

Cupric     chromite     basic,     5CuO,     4Cr2O3. 
(Wohler,  Z.  phys.  Ch.  1908,  62.  445.) 

Cupric  chromite,  CuCr2O4. 

Not  attacked  by  HNO3+Aq.  (Persoz,  A. 
ch.  (3)  25.  283.) 

Not  attacked  by  cone.  HC1. 

Insol.  in  dil.  acids.  (Wohler,  Z.  phys. 
Ch.  1908,  62.  446.) 

CuO,  3Cr203.  (Rosenfeld,  B.  1879,  12. 
958.) 

Glucinum  chromite,  GlCr2O4. 

Insol.  in  H2O.    (Mallard,  C.  R.  105.  1260.) 

Iron  (ferrous)  chromite  (chrome  iron  ore). 

See  Chromite,  aluminum  ferrous  magne- 
sium. 

Iron  (ferroferric)  chromite,  FeO,  Fe203,  Cr2O3. 
Not  attacked  by  HCl+Aq.     (Ebelmen.) 

Iron  (ferrous)  magnesium  chromite. 

Insol.  in  HCl+Aq.  Scarcely  attacked  by 
H2S04. 

Lead  chromite,  PbCr2O4. 

Ppt.  Insol.  in  KOH+Aq.  (Chancel, 
C.  R.  43.  927.) 

Lithium  chromite,  Li2Cr2O4. 

Very  si.  sol.  in  acids.  (Weyberg,  C.  C. 
1906,  II.  1659.) 

Magnesium  chromite,  MgO,  2Cr2O3. 

Insol.  in  H2O.  (Nichols,  Sill.  Am.  J.  (2) 
47.  16.) 

MgCr2Os.  Insol.  in  acids  or  alkalies,  ex- 
cept boiling  H2SO4.  (Schweitzer,  J.  pr.  39. 
259.) 

Could  not  be  obtained.  (Viard,  Bull.  Soc. 
(3)  5.  934.) 


Easily   attacked    by   boiling   H2SO4+Aq. 
Less  easily  by  HC1  or  HF+Aq  not  at- 
cked  by  boilii 
1896,  123.  886.) 


ly  fa- 
tacked  by  boiling  HNO3.     (Dufau,   C.   R. 


2MgO,  Cr2O3.  Insol.  in  H2O  or  acids. 
(Nichols.) 

5MgO,  4Cr2O3.  Insol.  in  acids.  (Viard, 
C.  R.  112.  1003.) 

3MgO,2Cr2O3.    As  above.    (V.) 


COBALT, AMMONIA  COMPOUNDS 


279 


Manganese  chromite,  MnCr2O4. 

Entirely  insol.  in  acids.  (Ebelmen,  A. 
ch.  (3)  33.  44.) 

Zinc  chromite,  ZnCr2O4. 

Insol.  in  acids  and  alkalies,    ("faard,  C.  R. 

109.  142.) 

+ zH2O.    (Chancel,  C.  R.  43.  927.) 
3ZnO,  2Cr2O3.    As  above.     (Viard,  C.  R. 

112.  1003.) 

6ZnO,  5Cr203.    As  above.    (V.) 

8ZnO,    3Cr2O3.      (Groger,    M.    1904,    25, 

520.) 

Chromovanadic  acid. 

Ammonium  chromovanadate,   2(NH4)2O, 

2Cr03,  V205+7H20. 
Sol.  in  H20.    (Ditte,  C.  R.  102.  1105.) 

Chromyl  amide,  CrO2  (NH2)2. 
Sol.  in  H2O.    (Ohly,  C.  N.  1899,  80. 134.) 

Chromyl  sw&chloride,  (CrO2)5Cl6. 

Deliquescent,  sol.  in  H2O  with  decomp., 
insol.  in  dry  ether.  (Pascal,  C.  R.  1909, 
148,  1463.) 

Chromyl     chloride      (chlorochromic     acid) 
CrO2Cl2. 

Decomp.  by  H2O  with  evolution  of  much 
heat.  Sol.  in  glacial  acetic  acid  without  de- 
composition. 

Sol.  in  CC14,  C6H6,  (mol.  wt.  det.).  (Oddo, 
Gazz.  ch.  it.  1899,  29.  (2)  318;  Chem.  Soc. 
1900,  78.  (2)  75.) 

Tnchromyl  chloride,  Cr3O6Cl2. 

Deliquescent.  Sol.  in  H2O  with  gradual 
decomposition.  Sol.  in  cone.  HCl+Aq. 
(Thorpe,  Chem.  Soc.  (2)  8.  31.) 

Scarcely  sol.  in  CS2. 

Sol.  in  alcohol  and  ether.  (Rawson,  C.  N. 
1889.  59.  185.) 

Chromyl  chic  rides. 
From  Cr2O3. 
See  Chromium  oxy chlorides. 

Chromyl  chloride  nitrogen  fe/roxide, 

Cr6Cl607,  2N02. 

Sol.  in  H2O  with  decomp.  (Thomas,  C.  R. 
1899,  129.  828.) 

Chromyl  fluoride,  CrO2F2. 

Decomp.  by  H2O  with  evolution  of  heat. 
(Oliveri,  Gazz.  ch.  it.  16.  218.) 

Clay. 

See  Silicate,  aluminum,  A12O3,  SiO2-f- 
2H20. 


Cobalt,  Co. 

Not  attacked  by  H2O. 

Sol.  in  dil.  HC1,  or  H2SO4.  or  HNO8+Aq. 
Cone,  hot  H2SO4,  and  HNO3  decomp.  with 
evolution  of  SO2  or  NO  gas. 

Exists  also  in  passive  state.  See  Iron. 
(Nickles,  J.  pr.  61.  186.) 

Sol.  in  cone.  KOH-j-Aq  when  in  finely 
divided  state.  (Winkler,  J.  pr.  91.  211.) 

Sol.  in  NH4OH+Aq  in  presence  of  air. 
(Hodgkinson  and  Bellairs,  C.  N.  1895,  71.  73.) 

Cobalt  ammonia  compounds. 

See — 

Anhydrooxycobaltamine   compounds, 

[Co(NH3)5]2[g|OH)]x4. 

Bromotetramine   cobaltic   compounds, 
BrCo(NH3)4X2. 

Bromopurpureocobaltic  compounds, 
BrCo(NH3)5X2. 

Carbonatotetramine  cobaltic  compounds,. 
(C03)Co(NH3)4X. 

Chlorotetramine     cobaltic     compounds, 
ClCo(NH3)4X2 

Chloropurpureocobaltic   compounds, 
ClCo(NH3)5X2 

Croceocobaltic  compounds, 
Co(NH3)4(N02)2X. 

Decamine    cobaltic   sulphite, 
Co2(NH3)10(S03)3. 

Diamine  cobaltic  nitrites, 
Co(NH3)2(NO2)4M. 

Dichrocobaltic  compounds,  Co(NH3)sX8. 

Flavocobaltic   compounds, 
(NO2)2Co(NH3)4X. 

Fuscocobaltic  compounds, 
(OH)Co(NH3)4X2. 

lodotetramine  cobaltic  compounds, 
ICO(NH3)4X2. 

Luteocobaltic  compounds,  Co(NH3)6X8. 

Melanocobaltic  compounds, 
[Co(NH3)3Cl2]2,  NH2C1. 

Nitratotetramine  cobaltic  compounds, 
(N03)Co(NH3)4X2. 

Nitratopurpureocobaltic  compounds, 
(NO)3Co(NH3)6X2. 

Nitritocobaltic  compounds, 
(N02)Co(NF3)6X2. 

Octamine  cobaltic  compounds, 
Co2(NH3)8  X,. 

(=Tetramine  cobaltic  compounds, 
Co(NH8)<X8. 

Oxycobaltamine  compounds, 
Co2(NH3),0(OOH)X4. 

Praseocobaltic  compounds,  Co(NH8)4X8. 

Purpureocobaltic   compounds, 
Co(NH3)6X3. 

Roseocobaltic  compounds, 
Co(NH3)6(OH2)X8. 

Sulphatotetramine  cobaltic  compounds, 
(S04)Co(NH3)4X. 

Sulphatopurpureocobaltic  compounds, 
(S04)Co(NH3)6X. 


280 


COBALT  ARSENIDkE 


"  Tetramine  cobaltic  "  compounds, 

Co(NH3)2X3. 

Xanthocobaltic  compounds, 
(N02)Co(NH8)6X2. 

Cobalt  arsenide,  CoAs. 

As  Co3As2.  (Ducelliez,  C.  R.  1908,  147. 
425.) 

CoAs2.  As  Co3As2.  (DuceUiez,  C.  R. 
1908,  147.  425.) 

Co2As3.  As  Co3As2.  (Ducelliez,  C.  R. 
1908,  147.  425.) 

Co3As2.  Very  si.  attacked  by  hot  cone. 
HC1,  less  by  H2SO4.  .Easily  sol  in  HNO3 
and  aqua  regia.  SI.  attacked  by  fused  al- 
kalies and  alkali  carbonates.  (Ducelliez, 
C.  R.  1908,  147.  425.) 

CoAs3.  Min.  Skutterudite.  Sol.  in  HNO8 
-f-Aq,  with  separation  of  As2O3. 

Cobalt  arsenide  sulphide,  CoAs2,  CoS2. 

Min.  Cobaltite.  Sol.  in  HNO3+Aq,  with 
separation  of  S  and  As2O8. 

Glaucodote.  Completely  sol.  in  HNO3  + 
Aq. 

Cobalt  azoimide,  basic,  Co(OH)N3. 

Insol.  in  H2O. 

Sol.  in  HN3+Aq.  (Curtius,  J.  pr.  1898,  (2) 
58.  300.) 

Cobalt  potassium  azoimide,  KN3,  Co(N8)2. 

Sol.  in  H2O ;  Aq.  solution  decomp.  on  boiling. 
(Curtius,  J.  pr.  1898,  (2)  68.  301.) 

Cobalt  boride,  Co2B. 

Attacked  by  HNO3.  (Jassonneix,  C.  R. 
1907,145.240,) 

CoB.  Decomp.  by  moist  air  and  by  al- 
kali nitrates,  chlorates,  hydroxides  and  car- 
bonates; decomp,  by  steam  at  red  heat  and 
by  acids.  (Moissan,  C.  R.  1896,  122.  425.) 

Not  attacked  by  HC1;  rapidly  attacked 
t>y  HNO8.  Not  attacked  by  dil.  but  decomp. 
by  cone.  H2SO4.  Rapidly  attacked  by  aqua 
regia.  (Moissan,  A.  ch.  1896,  (7)  9. 272.) 

CoB2.    (Jassonneix,  C.  R.  1907, 146.  241.) 

Cobaltous  bromide,  CoBr2. 

Deliquescent.  Sol.  in  H2O,  alcohol,  and 
ether. 

Sat.  CoBr2+Aq  contains  at: 
59°         75°         97° 
66.7        66.8        68.1%  CoBr2. 
<fitard,  A.  ch.  1894,  (7)  2.  542.) 

Nearly  insol.  in  AsBr3.  (Walden,  Z.  anorg. 
1902,  29.  374.) 

Sol.  in  S02C1(OH).    (Walden.) 

Sol.  in  quinoline.  (Beckmann  and  Gabel, 
Z.  anorg.  1906,  61.  236.) 

Ig.  CoBr2  is  sol.  in  9.74g.  methyl  acetate 
at  18°.  Sp.  gr.  1874°  of  sat.  solution  =  1.013. 
{Naumann,  B.  1909,  42.  3792.) 


Difficultly  sol.   in  ethvl   acetate.     (Nau- 
mann, B.  1910,  43.  314.) 
Sol.  in  acetone.     (Eidmann,  C.  C.  1899, 

11.  1014;  Naumann,  B.  1904,  37.  4328.) 
Mol.     weight    determined     in    pyridine. 

(Werner,  Z..  anorg.  1897,  15.  24.) 

+2,  and  6H2O.    (Hartley,  Chem.  Soc.  (2) 

12.  214.) 

Cobaltous    hydrazine    bromide    hydrazine. 

2CoBr2,  4N2H4HBr,  N2H4(?).    ' 
Sol.  in  H2O  with  decomp.    (Ferratini,  C.  A. 
1912.  1613.) 

Cobaltous   mercuric   bromide,   basic, 

CoBr2,  HgBr2,  6CoO+20H2O. 
(Mailhe,  A.  ch.  1902,  (7)  27.  369.) 

Cobalt  stannic  bromide. 
See  Bromostannate,  cobalt. 

Cobaltous  bromide  ammonia,  CoBr2,  6NH3. 

Sol.  in  H2O  with  residue  of  cobalt  hydrox- 
ide. (Rammelsberg,  Pogg.  55.  245.) 

Cobaltous  bromide  hydrazine,  CoBr2,  2N2H4. 
Decomp.  by  boiling  with  H2O.    (Franzen, 
Z.  anorg.  1908,  60.  270.) 

Cobalt  carbonyl,  Co(CO)4. 

Insol.  in  H2O.  More  or  less  sol.  in  CS2, 
ether,  alcohol  and  Ni(CO)4.  Relatively 
stable  with  non-oxidizing  acids.  Quickly 
decomp.  by  oxiding  acids.  (Mond,  Hirtz 
and  Cowap,  C.  N.  1908,  98.  165.) 

Cobaltous  chloride,  CoCl2. 

Deliquescent.  Sol.  in  H2O  with  evolution 
of  heat.  100  pts.  H2O  dissolve  43.3  pts.  CoCl2 
at  0°.  (Engel,  A.  ch.  (6)  17.  355.) 

100  pts.  sat.  CoCla+Aq  at  t°  contain  pts. 
CoCl2. 


t° 

Pts. 
CoCh 

t° 

Pts. 
CoCh 

t 

Pts. 
CoCls 

-22 

*-  4 
+  7 
11 
12 

24.7 
28.0 
31.2 
31.3 
32.5 

25 
34 
41 
45 
49 

34.4 
37.5 
39.8 
41.7 
46.7 

56 
78 
94 
96 
112 

48.4 
48.8 
50.5 
51.2 
52.3 

(fitard,  C.  R.  113.  699.) 

Sp.  gr.  of  CoCl2+Aq  containing— 
5  10          12          20          25%CoCl2. 

1.0496   1.0997   1.1579   1.2245    1.3002 

Sat.  solution,  1.3613. 
(Franz,  J.  pr.  (2)  5.  284.) 

Sp.  gr.  of  CoCl2+Aq  containing  in  1000  g. 
CoCl2+6H20—     ' 


119 
1.055 


H20,  g. 

238       357       476       594 
1.101    1.141    1.177    1.209 
833         952          1071        1190 
1.238     1.264       1.287      1.309 


COBALTOUS  CHLORIDE 


281 


Containing  g.  CoCl2  (anhydrous)— 
65g.(  =  ^mol.)  130    195     260     325     390 
1.058  1.1121.1641.2131.2601.304 

(Gerlach,  Z.  anal.  28.  466.) 

Sp.  gr.  of  CoCl2+Aq  at  room  temp,  con- 
taining: 

7.97        14.858      22.27%  CoCl2. 
1.0807       1.1613       1.2645 
(Wagner,  W.  Ann.  1883,  18.  267.) 

Sp.  gr.  of  CoCl2+Aq  at  20°  containing  M 
g  mols.  of  salt  per  liter. 

M  0.01         0.025          0.05         0.075 

Sp.  gr.  1.001159  1.003052  1.006065  1.009190 


M  0.10 

Sp.  gr.  1.012386 


0.25 
1.03049 


0.50 
1.05492 


0.75 
1.09118 


M  1.0  1.5  2.0 

Sp.  gr.    1.11847     1.17502     1.23637 

(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38,711.) 

Sp.  gr.  of  CoCl2+Aq.  at  25°. 


Concentration  of 
CoClz+Aq. 

Sp.  gr. 

1  —  normal 

Vr-      " 

'/4-           " 

Vs-        " 

1.0571 
1.0286 
1.0144 
1.0058 

(Wagner,  Z.  phys.  Ch.  1890,  5.  37.) 


Solubility  in  HCl+Aq  at  0°. 

CoCl2  in  nigs,  in  10  ccm.  of  solution. 
HCl  =  mols.  HC1  in  mgs.  in  ditto.  H2O 
=  g.  H20. 


CoCh 
2 

HCl 

CoCl2 
+HC1 

Sp.  gr. 

H2O 

62.4 

0 

62.4 

1.343 

9.36 

58.525 

3.7 

62.2 

.328 

9.34 

50.8 

11.45 

62.25 

.299 

9.27 

37.25 

25.2 

62.45 

.248 

9.13 

12.85 

55  0 

67.85 

.167 

4.75 

74.75 

79.50 

.150 

8.46 

12.0 

104.5 

116.5 

.229 

7.5 

25.0 

139.0 

164.0 

1.323 

(Engel,  A.  ch.  (6)  17.  355.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Sol.  in  alcohol. 

Sat.  solution  in  alcohol  (0.792  sp.  gr.)  con- 
tains 23.66  %  CoCl2  and  has  sp.  gr.  =  1.0107. 
(Winkler,  J.  pr.  91.  209.) 

Very  sol.  in  ether. 

100  pts.  absolute  ether  dissolve  only  0.021  g. 
CoCl2.  (Bodtker,  Z.  phys.  Ch.  1897,  22. 
511.) 


100  g.  formic  acid  (95%)  dissolve  6.2  g. 

7. 
1117.) 


CoCl2  at  20.2°.     (Aschan,  Ch.  Z.  1913^  31 


Ig.  CoCl2  is  sol.  in  271g.  methyl  acetate 
at  18°.  Sp.  gr.  1874°  of  sat.  solution  =  0.938. 
(Naumann,  B.  1909,  42.  3791.) 

Difficultly  sol.  in  ethyl  acetate.  (Nau- 
mann, B.  1910,  43.  314.)  " 

100  pts.  acetone  dissolve  8.62  pts.  anhy- 
drous CoCl2.  (Krug  and  M'Elroy,  J.  Anal. 
Ch.  6.  184.) 

0.08  pts.  sol.  in  100  pts.  ethyl  acetate  at  14°. 
0.26  "  "  "  100  "  "  "  "  79°. 
9.11  "  "  "  100  "  acetone  "  0°. 

9.28    "       "  "  100  "         "  "22.5°. 

(Laszczynski,  B.  1894,  27, 2286.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899,  II. 
1014.) 

1  g.  CoCl2  is  sol.  in  36.4  g.  acetone  at  18°. 
Sp.  gr.  of  sat.  solution  18°/4°  =  0.825.  (Nau- 
mann, B.  1904,  37.  4334.) 

100  g.  acetonitrile  dissolve  4.08  g.  CoCl2  at 
18°.  (Naumann  and  Schier,  B.  1914,  97.  249.) 

Sol.  in  quinoline.  (Beckmann  and  Gabel, 
Z.  anorg.  1906,  51.  236.) 


Solubility  in  pyridine  at  t°. 

t° 

G.  Cods  sol.  in 
100  g.  pyridine 

Solid  phase 

—50.3 

0.4200 

—45.0 

0.4204 

—30.0 
—19  6 

0.4224 
0.4227 

CoC)2,  6C6H6N 

—10.0 

0.4329 

0 

0.4326 

+23.0 

0.572 

25.0 

0.578 

34.6 

0.755 

37.6 

0.760 

44.6 

0.959 

47.2 

.029 

CoCl2;  4C5H6N 

51.0 

.122 

55.0 

.206 

60.0 

.342 

64.2 

.483 

68.0 

.597 

74.8 

2.079 

78.2 
79.8 

2.330 

2.488 

CoCl2,  2C6HBN 

88.0 

3  397 

96  5 

7.817 

98.8 
106.0 

8.862 
14.340 

CoCl, 

110.0 

16.500 

(Pearce  and  Moore,  Am.  Ch.  J.  1913,  50.  226.) 

Mol.  weight  determined  in  piperidine, 
and  pyridine.  (Werner  Z.  anorg.  1897,  15. 
18  and  23.) 

Sol.  in  urethane.  (Castoro.  Z.  anorg. 
1899,  20.  61.) 

+H20. 


282 


COBALTCHJS  HYDRAZINE  CHLORIDE 


+2H2O.  Very  deliquescent.  (Bersch 
J.  B.  1867.  291.) 

17.16  pts.  sol.  in  100  pts.  acetone  at     0°. 

17.06  "  "   100     "  "       "    25°. 

(Laszczynski,  B.  1894,  27.  2287.) 

+4H2O.     Deliquescent.     (Bersch.) 

+6H2O.  Not  deliquescent.  Easily  sol 
in  H2O. 

Solubih'ty  of  CoCl2+6H2O  in  ethyl  alcohol 
-f-Aq  at  11.5°  under  addition  of  increasing 
amounts  of  CoCl2. 

P  =  Percent  of  alcohol  by  volume. 

G  =  Grams  of  CoCl2  added. 

Cc  =  Grams  of  CoCl2  in  5  cc.  of  the  solution. 

Cw  =  Grams  of  water  in  5  cc.  of  the  solution, 
calculated  from 

(1)  the  water  content  of  the  alcohol. 

(2)  the  water  of  crystallization  which  had 

gone  into  solution. 

(3)  the  water  held  mechanically  in  CoCl 

+6H2O. 


p 

G 

Cw 

Cc 

91.3 

0.0 

1.325 

1.168 

98.3 

0.0 

1.134 

1.214 

98.3    ' 

0.0 

1.068 

1.181 

99.3 

0.0 

1.045 

1.199 

t( 

0.194 

0  899 

1  204 

u 

0.40C 

0.829 

1.325 

K 

0.612 

0.764 

1.459 

(( 

0.813 

0.688 

1.568 

(I 

1.022 

0.634 

1.713 

(( 

1.240 

0.553 

1.831 

(S 

1.446 

0.483 

1.943 

11 

0.650 

0.5CO 

2.186 

(Bodtker,  Z.  phys.  Ch.  1897,  22.  508.) 

Easily  soluble  in  absolute  ethyl  alcohol. 
100  pts.  absolute  alcohol  dissolve  at  room 
temperature  56.20  pts.  CoCl2.  Water  pre- 
cipitates CoCl2+6H2O  from  a  solution  of 
CoCl2  in  absolute  alcohol.  (Bodtker.) 

100  pts.  absolute  ether  dissolve  0.291g. 
CoCl2+6H2O.  (Bodtker,  Z.  phys.  Ch.  1897, 
22.  511.) 

Anhydrous  ethylene  glycol  dissolves 
10.6%  CoCl2+6H26  at  16.4°.  (de  Coninck, 
Chem.  Soc.  1904,  86,  (2)  741.) 

Cobaltous  hydrazine  chloride, 

CoCl2,  2N2H4HC1+2^H2O. 
Sol.  in  H2O.    (Ferratini,  C.  A.  1912.  1613.) 

Cobaltous   iodine   chloride,   CoCl2,   2IC13  + 

8H2O. 

Hygroscopic.  Decomp.  by  H2O.  CC14 
separates  IC13.  (Weinland  and  Schlegel- 
milch,  Z.  anorg.  1902,  30.  137.) 

Cobalt  lithium  chloride,  CoCl2,  LiCl+3H2O. 
Very  deliquescent.  Sol.  in  H2O  with  de- 
comp.  Sol.  in  LiCl+Aq  without  decomp. 
Sol.  in  alcohol  without  decomp.  (Chassevant, 
A.  ch.  (6)  30.  27.) 


Cobaltous   mercuric  chloride    basic,  CoCl2, 

HgCl2,  6CoO+20H2O. 
(Mailhe,  A.  ch.  1902,  (7)  27.  369.) 

Cobaltous  mercuric  chloride,  CoCl2,  HgCl2. 
Very  deliquescent,     (v.  Bonsdorff.) 

Cobaltous  thallic  chloride,  2T1C13,  CoCI2-f- 

8H2O. 

Hydroscopic;    can    be    cryst.    from    H2O. 
(Gewecke,  A.  1909,  366.  222.) 

Cobaltous  tin  (stannic)  chloride,  CoCl2,  SnCl4 

+6H2O. 
See  Chlorostannate,  cobaltous. 

Cobaltous  chloride  ammonia,  CoCl2,  2NH8. 
Decomp.  by  H2O.    (F.  Rose.) 
CoCl2,   4NH3.     Decomp.   by   H2O.     (H. 


CoCl2,  6NH3.  Decomp.  by  H2O.  Sol.  in 
dil.  NH4OH+Aq  with  ease,  but  difficultly  in 
cone.  NH4OH+Aq.  Insol.  in  absolute 
alcohol.  (Fremy.) 

Cobaltous  chloride  hydrazine,  CoCl2,  2N2H4. 

Insol.  in  cold  H2O. 

Slowly  decomp.  by  cold,  rapidly  by  hot 
H2O. 

Easily  sol.  in  dil.  acids  and  NH4OH+Aq. 
(Franzen,  Z.  anorg.  1908,  60.  270.) 

Cobaltous  chloride  hydroxylamine, 

CoCl2,  2NH2OH. 
Decomp.  in  the  air;  sol.  in  H2O.     (Feldt. 
B.  1894,  27.  403.) 

Cobaltic  chloride  hydroxylamine, 
CoCl3,  6NH2OH. 

Insol.  in  alcohol. 

Sol.  in  acidified  H2O  without  decomp.; 
sol.  in  cone.  H2SO4  without  decomp. 
(Feldt,  B.  1894,  27.  404.) 

Cobaltous  fluoride,  CoF2. 

SI.  sol.  in  H2O;  insol.  in  alcohol  and  ether; 
slowly  attacked  by  cold  HC1,  H2SO4,  or  HNO3 
+Aq.  (Poulenc,  C.  R.  114.  1429.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  29.  827.) 

+2H2O.  Sol.  in  a  little  H2O  without  de- 
comp. Decomp.  into  oxyfluoride  by  boiling 
with  much  H2O.  Sol.  in  HF+Aq.  '(Ber- 
zelius.) 

+4H2O.    Two  modifications. 
Solubility  of  a  mod.  at  ?°=  2.2328  % 
"  j3    "       «  "  =2.3203  %. 
(Costachescu,  Ann.  Sci.  Univ.  Jassy,   1912, 
7,  1,  10.) 

obaltic  fluoride,  CoF3. 
Sol.   in   cone.   H2SO4.      (Barbieri,    Chem. 
Soc.  1905,  88,  (2)  393.) 


COBALTOUS IODIDE 


283 


Cobaltous  hydrogen  fluoride,  CoF2,  5HF  + 
6H2O. 

Easily  sol.  in  H2O  and  dil.  acids. 

Sol.  in  NH4OH-j-Aq  with  decomp.  (Bohm, 
Z.  anorg.  1905,  43.  330.) 

Cobalt  columbium  fluoride. 
See  Fluocolumbate,  cobalt. 

Cobaltous  iron  (ferric)  fluoride, 

CoF2,  FeF3+7H2O. 

Sol.  in  dil.  HF+Aq.  (Weinland,  Z.  anorg. 
1899,  22.  269.) 

Cobaltous  manganic  fluoride,  2CoF2,  Mn2FG 

+8H20. 
(Christensen,  J.  pr.  (2)  34.  41.) 

Cobalt  molybdenyl  fluoride. 
See  Fluoxymolybdate,  cobalt. 

Cobaltous  potassium  fluoride,  CoF2,  KF. 

SI.  sol.  in  H2O;  less  in  ethyl  or  methyl 
alcohol;  insol.  in  amyl  alcohol  or  benzene. 
Decomp.  by  hot  H2SO4.  (Poulenc,  C.  R.  114. 
747.) 

+H2O.  SI.  sol.  in  H2O.  (Wagner,  B.  19. 
896.) 

CoF2,  2KF. 

Cobaltous  sodium  fluoride,  CoFa,  NaF+H2O. 
Sol.  in  H2O.    (Wagner,  B.  19.  896.) 

Cobaltous  stannic  fluoride. 
See  Fluostannate,  cobaltous. 

Cobalt  vanadium  fluoride. 
See  Fluovanadate,  cobalt. 

Cobaltous  hydroxide,  CoO2H2. 

Insol.  in  H2O.  Sol.  in  acids.  Insol.  in 
KOH+Aq.  Sol.  in  ammonium  sulphate, 
chloride,  nitrate,  or  succinate+Aq.  (Brett.) 

Sol.  in  warm  acetic  acid;  insol.  in  NH4OH 
+Aq  and  cold  NH4Cl+Aq,  but  sol.  in 
warm  NH4Cl+Aq.  (de  Schulten,  C.  R.  109. 
266.) 

Insol.  in  H2O  and  dil.  KOH+Aq;  some- 
what sol.  in  cone.  KOH+Aq;  easily  sol.  in 
NH4  salts+Aq.  (Fresenius.) 

Easily  sol.  in  KCN+Aq.    (Rodgers,  1834.) 

Sol.  in  cone.  K2CO8+Aq.     (Gmelin.) 

Not  pptd.  by  KOH+Aq  in  presence  of 
H2C4H4O6  or  NH4  citrate.  (Spiller.) 

Sol.  in  large  amt.  in  boiling  NH4SCN+Aq. 
(Grossmann,  Z.  anorg.  1908,  58.  269.) 

Insol.  in  methyl,  or  amyl  amine  +Aq. 
(Wurtz.) 

Many  non-volatile  organic  substances  pre- 
vent its  pptn. 

Cobaltic  hydroxide,  3Co2O3,  2H2O. 
(Mills,  Phil.  Mag.  (4)  35.  257.) 
Co2O«,  2H2O.  Decomp.  by  HCl+Aq; 


gives  brown  solutions  with  cold  HNOj  or 
H2SO4+Aa,  which  soon  decomp.  (Wernicke, 
Pogg.  141.  120.) 

Co2O6H6  =  Co2O3, 3H2O.  Sol.  in  warm  HC1, 
HNO3,  and  H2SO4,  with  decomp.  (Proust.) 

Sol.  in  cold  H3PO4,  H2SO4,  HNO3,  or  HC1+ 
Aq,  but  decomp.  on  standing  or  warming. 
(Winkelblech.) 

Sol.  in  racemic,  tartaric,  oxalic,  or  citric 
acid  as  cobaltous  salt. 

Sol.  in  cone,  acetic  acid  without  immediate 
decomp.  (Remele).  Solution  is  not  decomp. 
by  boiling.  Sol.  in  warm  sat.  (NH4)2C2O4  + 
Aq  with  decomp. 

Not  attacked  by  cold  or  hot  NH4OH+Aq. 

Insol.  in  boiling  NH4Cl+Aq. 

Sol.  when  freshly  pptd.  in  fNH4)2SO8  + 
Aq.  (Geuther,  A.  128.  157.) 

Cobaltocobaltic  hydroxide,  Co3O4,  3H2O. 

Insol.  in  H2O.  Sol.  in  oxalic  acid;  solution 
decomp.  by  heat.  Sol.  in  HCl+Aq  with 
evolution  of  Cl.  (Gibbs  and  Genth,  Sill.  Am. 
J.  (2)  23.  257.) 

Co3O4,  7H2O.  Sol.  in  weak  acids,  especially 
HC2H3O2  without  decomp.  (Fremy.) 

Co6O7,  6H2O.  Min.  Hetewgenite.  Sol.  in 
dil.  HCl+Aq  with  evolution  of  Cl. 

Cobaltous  iodide,  CoI2. 

Deliquescent,  and  very  sol.  in  H2O. 

100  pts.  sat.  CoI2+Aq  at  t°  contain 
pts.  CoI2. 


t 

Pts. 

Col2 

t° 

Pts. 
CoI2 

t° 

Pts. 
Col: 

—22 

.     Q 

2 

+  9 

52.4 
56.7 

58.7 
61.4 

14 
25 
34 
46 

61.6 
66.4 
73.0 
79.0 

60 
82 
111 
156 

79.2 
80.7 
80.9 
83.1 

(fitard,  C.  R.  113.  699.) 

Sol.  in  SO2(OCH3)2.  (Walden,  Z.  anorg. 
1902,  29.  388. 

Sol.  in  SOC12.  (Walden,  Z.  anorg.  1900, 
25.  216.) 

Sol.  in  POC13.  (Walden,  Z.  anorg.  1900, 
25.  212.) 

Sol.  in  S2C12.  (Walden,  Z.  anorg.  1900,  25. 
217.) 

Nearly  insol.  in  AsBr3.  (Walden,  Z.  anorg. 
1902,  29.  374.) 

Sol.  in  AsCls.  (Walden,  Z.  anorg.  1900, 
25.  214.) 

Easily  sol.  in  alcohol. 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014.)  (Naumann,  B.  1904,  37.  4328.) 

Sol.  in  quinoline.  (Beckmann  and  Gabel, 
Z.  anorg.  1906,  61.  236.) 

Sol.  in  methyl  acetate.  ( Naumann,  B.  1909, 
42,  3790.) 

+2H20. 

+4H2O.    Very  deliquescent.     (Etard.) 


284 


COB ALTO US  LEAD  IODIDE 


+6H2O.  (Hartley,  Chem.  Soc.  (2)  12 
214.) 

+9H2O.  Very  hydroscopic.  (Bolschakoff, 
C.  C.  1898,  II.  660.) 

Cobaltous  lead  iodide,  2  CoI2,  PbI2+3H2O 

Decomp.  by  F2O.    (Mosnier,  A.  ch.  1897, 

(7)  12.  412.) 

Cobaltous  mercuric  iodide,  CoI2,  HgI2  + 
6H20. 

Partially  decomp.  by  H2O. 

Sol.  in  alcohol  and  acetone.  (Dobroserdoff, 
C.  C.  1901,  II.  332.) 

CoI2, 2HgI2+6H20.  Decomp.  by  H2O;  sol. 
in  alcohol  and  acetone.  (Dobroserdoff,  C.  C. 
1901,  II.  332.) 

Cobaltous  iodide  ammonia,  CoI2,  4NH3. 

Decomp.  by  H2O.  Sol.  in  NH4OH+Aq. 
(Rammelsberg,  Pogg.  48.  155.) 

Col2,  6NH3.  Insol.  in  NH4OH+Aq. 
(Rammelsberg.) 

Cobaltous  iodide  hydrazine,  CoI2,  2N2H4. 

SI.  sol.  in  H2O.  Easily  sol.  in  acids. 
(Franzen,  Z.  anorg.  1911,  70.  147.) 

Cobaltic  octamine  compounds. 
See  Octamine  cobaltic  compounds. 

Cobaltous  oxide,  CoO. 

Insol.  in  H2O.  Easily  sol.  in  dil.  or  cone. 
HC1  or  HNOs+Aq.  Slowly  sol.  in  cold,  but 
easily  in  hot  dil.  H2SO4+Aq,  acetic,  or 
tartaric  acid  +Aq.  Insol.  in  NH4OH+Aq. 
Sol.  in  hot  NH4C1  +Aq,KOH,  or  NaOH+Aq. 
(Rose.) 

Insol.  in  NH4Ct  or  NH4N03+Aq.  (Brett, 
1834.) 

Insol.  in  K2C03-fAq.  Sol.  in  boiUng  Ce 
and  Ni  nitrates  +Aq,  with  pptn.  of  the  ox- 
ides. (Persoz.) 

Easily  sol.  in  dil.  acids,  even  tartaric. 
acetic,  and  oxalic  acids.  Not  attacked  by 
NH4OH+Aq.  Sol.  in  13%  NH4Cl+Aq 
with  evolution  of  NH3;  also  in  NH4SCN-f-Aq. 
Sol.  in  warm  cone.  NaOH,  and  KOH+Aq. 
(Zimmerman,  A.  232.  324.) 

Solubility  in  (calcium  su  crate +sugar)  +Aq. 

1  1.  solution  containing  418.6  g.  sugar  and 
34.3  g.  CaO  dissolves  1.56  g.  CoO;  1  1.  solu- 
tion containing  296.5  g.  sugar  and  24.2  g. 
CaO  dissolves  0.29  g.  CoO.  (Bodenbender, 
J.  B.  1866.  600.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

See  also  Cobaltous  hydroxide. 

Cobaltic  oxide,  Co203. 

Decomp.  by  most  acids,  even  in  the  cold, 
with  formation  of  cobaltous  salts.  Sol.  in 
acetic  acid  without  immediate  decomp. 

See  also  Cobaltic  hydroxide. 


Cobaltocobaltic  oxide,  Co3O4  =  CoO,  Co202. 

Insol.  in  boiling  cone.  HC1,  HNO3,  or  aqua 
regia.  Sol.  by  long  standing  with  H2SO4. 
(Gibbs  and  Genth,  Sill.  Am.  J.  (2)  23,  257.) 

See  also  Cobaltocobaltic  hydroxide. 

Co4O5=2CoO,  Co2O3. 

Co6O7=4CoO,  Co2O3.  Not  attacked  by 
boiling  dil.  HNO3  or  H2SO4+Aq.  (Beetz.') 

Co8O9  =  6CoO,  Co203+20H2O.  Sol.  in  dil. 
acids,  with  residue  of  Co2O3,  which  dis- 
solves on  warming.  (Gentele,  J.  pr.  69.  131.) 

H-8H2O.    As  above.    (Gentele.) 


Cobaltous  oxychloride,  CoCl2.  3CoO  + 


Ppt.  Very  si.  sol.  in  H2O.  (Habermann, 
M.  5.  432.) 

Cobaltous    oxychloride    hydroxylamhu  , 

CoOCl,  2NH2OH. 

Insol.  in  H2O;  unstable;  insol.  in  alcohol. 
(Feldt,  B.  1894,  27.  404.) 

Cobaltous  oxyfluoride,  CoO,  CoF2+F2O. 
Ppt.    (Berzelius,  Pogg.  1.  26.) 

Cobaltous  oxyiodide,  CoO,  CoI2. 
Insol.  in  H2O.    (Rammelsberg.) 

Cobaltous  oxysulphide,  CoO,  CoS. 

Cold  HCl+Aq  dissolves  out  CoO;  hot 
HCl+Aq  decomp.  with  evolution  of  H2S. 
(Arfvedson,  Pogg.  1.  64.) 

Cobalt  phosphide,  Co2P. 

Sol.  in  cone.  HNO3.  Slowly  attacked  by 
HC1  and  H2SO4.  (Maronneau,  C.  R.  1900, 
130.  658.) 

Sol.  in  HNO3,  aqua  regia,  and  in  fused 
alkalies.  (Granger,  Bull.  Soc.  1896,  (3)  15. 


Co2P3.  Insol.  in  HNO3  and  aqua  regia; 
stable  in  the  air  even  when  heated.  (Granger, 
Bull.  Soc.  1896,  (3)  15.  1087. 

Co3P2.  Insol.  in  cone.  HCl+Aq.  Sol.  in 
HNO3+Aq.  (Rose,  Pogg.  24.  332.) 

Cobalt  sw&selenide,  Co2Se. 

Sol.  in  bromine  water. 

Only  si.  attacked  by  boiling  fuming  HC1 
'Fonzes-Diacon,  C.  R.  1900,  131.  704.) 

/obalt  monoselenide,  CoSe. 
(Little,  A.  112.  211.) 

Cobalt  cfoselenide  CoSe2. 

Sol.inBr2+Aq. 

Only  si.  attacked  by  boiling  fuming  HC1 
(Fonzes-Diacon,  C.  R.  1900,  131.  705.) 


COBALTICYANIDE,  AMMONIUM  CALCIUM 


285 


Cobalt  sesgm'selenide,  Co2Se3. 

Sol.  inBr2+Aq. 

Only  si.  attacked  by  boiling  fuming  HC1 
(Fonzes-Diacon,  C.  R.  1900,  131.  704.) 

Cobalt  selenide,  Co3Se4. 

Sol.  inBr2+Aq. 

Only  si.  attacked  by  boiling  fuming  HC1 
(Fonzes-Diacon,  C.  R.  190,  131.  704.) 

Cobalt  silicide,  Co2Si. 

Sol.  in  HF  and  aqua  regia.  Insol.  in  cold 
H2O.  Decomp.  by  steam  at  red  heat.  Sol. 
in  fused  alkali  carbonates.  CVigouroux. 
C.  R.  1895,  121.  687.) 

CoSi.  Insol.  in  HNO3  and  H2SO4.  Sol 
in  aqua  regia  and  HC1,  and  in  fused  KOH. 
(Lebeau,  C.  R.  1901,  132.  557.) 

Not  attacked  by  dil.  or  cone.  HNO3,  or 
cone.  H2SO4.  Sol.  in  aqua  regia  and  in  cone. 
HC1. 

Not  attacked  by  dil.  alkali  hydroxides  + 
Aq.;  attacked  by  fused  alkali.  (Lebau,  Bull. 
Soc.  1901,  (3),  25.  540.) 

CoSi2.  SI.  sol.  in  hot  cone.  HC1  and  hot 
cone,  alkali  +  Aq.  Sol.  in  HF;  insol.  in 
HNO3  and  H2SO4.  (Lebeau,  C.  R.  19G2, 135. 
476.) 

Cobaltous  sulphide,  CoS. 

Anhydrous.  Easily  sol.  in  acids,  even 
HC2H3O2,  but  only  slowly  in  the  latter  case. 
(Hjortdahl,  C.  R.  65.  75.) 

Not  attacked  by  cold  dil.  HC1+ Aq.  (Ebel- 
men,  A.  ch.  (3)  25.  94.) 

Min.  Seypoorite. 

+zH2O.  1  1.  H2O  dissolve  41.62  +  10-6 
moles  CoS  at  18°.  (Weigel,  Z.  phys.  Ch. 
1907,  58.  294.) 

Sol.  in  cone,  mineral  acids;  very  si.  sol.  in 
cold  dil.  acids;  scarcely  sol.  in  acetic  acid. 
(Wackenroder.) 

Sol.  when  still  moist  in  SO2+Aq.  (Ber- 
thier.) 

Easily  sol.  in  HNO3,  but  only  very  si.  sol. 
in  HCl+Aq.  Not  pptd.  from  very  dil. 
acid  solutions  by  H2S. 

Insol.  in  H2O,  alkalies,  and  alkali  carbon- 
ates, or  sulphides  +  Aq.  (Fresenius.) 

Insol.  in  NH4C1,  and  NH4NO3+Aq. 
(Brett.) 

When  pptd.  by  (NH4)2S+Aq,  shows  a 
brown  colour  in  presence  of  200,000  pts.  H2O. 
(Pfaff.) 

Tartaric  acid,  etc.  does  not  hinder  the 
pptn.  by  rNH4)2S+Aq.  (Rose.) 

Sol.  in  potassium  thiocarbonate  +  Aq. 
(Rosenbladt,  Z.  anal.  26.  15.) 

Sol.  in  NaoSz  or  K2Sz+Aq.  (de  Koninck, 
Zeit.  angew.  Ch.  1891.  202.) 

Cobaltic  sulphide,  Co2S3. 

Partially  decomp.  by  HCl+Aq;  sol.  in 
HNO3+Aq  with  decomposition. 

SI.  attacked  by  HCl+Aq;  and  slowly  even 
by  aqua  regia.  (Schneider,  J.  pr.  (2)  9.  209.) 


Min.  Cobalt  pyrite. 

+zH2O.  Insol.  in  KCN+Aq.  (Fleck, 
J.  pr.  97.  303.)  More  sol.  in  HCl+Aq  than 
CoS2.  (Dingier,  Berz,  J.  B.  10.  139.) 

Cobaltoccbaltic  sulphide,  Co3S4. 

Min.  Linnceite.  Sol.  in  warm  HNO3+Aq, 
with  residue  of  S. 

Cobalt  ^'sulphide,  CoS2. 

Not  attacked  by  alkalies  or  acids  except 
HNO3  and  aqua  regia.  (Setterberg,  Pogg.  7. 
40.) 

Cobalt  sulphide,  Co4S3. 

Easily  sol.  in  hot  HC1  with  evolution  of 
H2S  (and  H2?).  (Proust.) 

Cobalt  potassium  sulphide,  K2CouSi0. 

Slowly  sol.  in  cold  HC1  and  aqua  regia. 

Quickly  sol.  in  warm  aqua  regia. 

Sol.  in  HF  and  H2SO4  only  on  warming. 

Insol.  in  (NH4)2S,  organic  acids,  alkalies, 
12%  HCl+Aq  and  KCN+Aq.  (Milbauer, 
Z.  anorg.  1904,  42.  447.) 

Cobalt  telluride,  CoTe. 
(Fabre,  C.  R.  105.  673.) 

Cobalt  decamine  sulphurous  acid. 
See  Decamine  cobaltisulphurous  acid. 

Cobaltic  acid. 

Potassium  cobaltate,  K2Co9Oi6+2H2O,  or 
3H2O. 

Insol.  in  H2O  (Pebal,  A.  100.  262),  but  de- 
comp. by  long  boiling.  Sol.  in  cone,  acids. 

K2O,  zCoO3.  Sol.  in  H2O.  (Winkler,  J. 
pr.  91.  351.) 

Does  not  exist.  (Donath,  W.  A.  B.  102,  2b. 
71.) 

Cobalticyanhydric  acid,  H3Co(CN)6+HH2O. 

Deliquescent.  Very  sol.  in  H2O  and  only 
si.  decomp.  on  boiling. 

Sol.  in  HCl+Aq  without  decomp.  even  on 
boiling.  SI.  sol.  in  cone.,  more  sol.  in  dil. 
HNOa+Aq.  Not  decomp.  by  boiling  cone. 
HNO3+Aq  or  aqua  regia.  Insol.  in  cone., 
si.  sol.  in  dil.  H2SO4+Aq.  Sol.  in  alcohol. 
Insol.  in  ether. '  (Zwenger,  A.  162.  157.) 

Ammonium  cobalticyanide,   (NH4)sCo(CN)6 


Very  sol.  in  H2O;  si.  sol.  in  alcohol. 

Ammonium  barium  cobalticyanide, 

NH4BaCo(CN)6+H2O. 
Sol.  inHsO.    (Weselsky.) 

Ammonium  calcium  cobalticyanide, 

NH4CaCo(CN)6+10H2O. 
Sol.  in  H2O. 


286 


COBALTICYANIDE,  AMMONIUM  LEAD 


Ammonium  lead  cobalticyanide, 

NHJPbCo(CN)6+3H2O. 
Sol.  in  8.31  pts.  H2O  at  18°,  and  si.  sol.  in 
93%  alcohol.     (Schuler.) 

Ammonium   mercuric   cobalticyanide, 

(NH4)6Co2Hg(CN)14+H20. 
Sol.  in  H2O  with  decomp. 
Insol.    in    alcohol.      (Soenderop,    Dissert. 
1899.) 

Ammonium  sodium  cobalticyanide, 

NH4Na2Co(CN)6. 
Only  si.  sol.  in  H2O.    (Weselsky,  B.  2.  598.) 

Ammonium  strontium  cobalticyanide, 

NH4SrCo(CN)6+9H2O. 
Sol.  inH2O.    (W.) 

Barium  cobalticyanide,  basic,  Ba3[Co(CN)6]2, 

BaO2H2. 

Not  very  stable.  Cannot  be  recryst.  with- 
out partial  decomp.  (W.) 

Barium   cobalticyanide,   Ba3[Co(CN)6l2  + 

10H2O. 

SI.  efflorescent.  Very  sol.  in  H2O.  Insol. 
in  alcohol. 

Barium    cobalticyanide    chloride, 

Ba3[Co(CN)6]2,  BaCl2  +  16H2O. 
Sol.  in  H2O  without  decomp.    (W.) 

Barium  lithium  cobalticyanide,  BaLiCo(CN)6 

+15H26. 

The  most.  sol.  of  the  double  cobalticy- 
anides.  (Weselsky.) 

Barium    potassium    cobalticyanide, 

BaKCo(CN)6+llH2O. 
Sol.  inH2O.    (W.) 

Bismuth  cobalticyanide  BiCo(CN)6. 

Ppt.  (Mathews,  J.  Am.  Chem.  Soc.  1900, 
22.  275.) 

-f  5H2O.  Moderately  stable  with  dil.  min. 
acids;  more  stable  with  cone,  acids  than  Cd 
or  Zn  comp. 

Decomp.  by  NH3  and  alkalies.  (Fischer 
and  Cuntze,  Ch.  Z.  1902,  26.  872.) 

Cadmium    cobalticyanide,    Cd3[Co(CN)6]2-f 


Attacked  by  strong  min.  acids  only  when 
hot.  Behaves  as  Zn  salt,  toward  cone. 
H2SO4  and  dil.  and  cone.  HC1. 

Insol.  in  K3Co(CN)6+Aq.  Sol.  in  NH4OH 
and  NH4Cl+Aq.  (Fischer  and  Cuntze,  Ch. 
Z.  1902,  26.  873.) 

Cadmium    potassium    cobalticyanide, 

KCdCo(CN)6. 

Not  attacked  by  H2O.  (Fischer  and 
Cuntze,  Ch.  Z.  1902.  26,  873.) 


Cadmium    sodium    cobalticyanide, 

NaCdCo(CN)6. 
(Fischer  and  Cuntze,  Ch.  Z.  1902,  26.  873.) 

Cadmium  cobalticyanide  ammonia, 

Cd3[Co(CN)6]2,  4NH3+2H20. 

(Fischer  and  Cuntze,  Ch.  Z.  1902,  26.  873.) 

Cd3[Co(CN)6]2,  5NH3+3H2O.  (Fischer 
and  Cuntze,  Ch.  Z.  1902,  26.  873.) 

Cd3[Co(CN)6]2,  7NH3.  (Fischer  and 
Cuntze,  Ch.  Z.  1902,  26.  873.) 

Cd3[Co(CN)6]2,  9NH3+2H2O.  (Fischer 
and  Cuntze,  Ch.  Z.  1902,  26.  873.) 

Calcium  potassium  cobalticyanide, 

CaKCo(CN)6+9H2O. 
Sol.  inH2O.    (W.) 

Cobaltous    cobalticyanide,    Co3[Co(CN)6]2  + 

14H20. 

Insol.  in  H2O  and  acids.  SI.  sol.  in  NH4OH 
+Aq.  Decomp.  by  KOH+Aq. 

Cupric      cobalticyanide,  Cu3[Co(CN)6]2  + 

7H2O. 

Insol.  in  H2O  and  acids.  Sol.  in  NH4OH  + 
+Aq. 

Cupric  cobalticyanide  ammonia, 

Cu3[Co(CN)6]2,  4NH3+7H2O. 
Sol.  in  H2O.    (Zwenger.) 

Lead  cobalticyanide,    basic,   Pb3[Co(CN)6]2, 

3PbO2H2+llH2O. 

Insol.  in  H2O  or  alcohol;  somewhat  sol.  in 
hot  Pb(C2H3O2)2+Aq.  (Schuler.) 

Lead  cobalticyanide,  Pb3[Co(CN)6]2+4H2O. 

Very  sol.  in  H2O.     Insol.  in  alcohol. 
(Zwenger.) 

+7H2O.  Sol.  in  1.77  pts.  H2O  at  18°,  and 
1.63  pts.  at  19.°  Insol.  in  absolute  alcohol. 
SI.  sol.  in  93%  alcohol.  (Schuler,  W.  A.  B. 
79.  302.) 

Lead  potassium  cobalticyanide,  PbKCo(CN)6 

+3H2O. 

Sol.  in  6.74  pts.  H2O  at  18°  and  much  more 
easily  in  hot  H2O.  Insol.  in  absolute,  si. 
sol.  in  93%  alcohol.  (Schuler.) 

Lead  cobalticyanide  nitrate,  Pb3[Co(CN)6]2, 
Pb(N03)2  +  12H20. 

Sol.  in  16.91  pts.  H2O  at  18°,  16.79  pts. 
at  19°,  and  much  less  hot  H2O. 

Nearly  insol.  in  93%  alcohol.     (Schuler.) 

Mercurous  cobalticyanide,  Hg3Co(CN)6. 

Ppt.  Decomp.  by  HC1.  Not  attacked  by 
cold,  but  by  hot  cone.  H2SO4.  Not  attacked 
by  HNO3,  acetic  or  oxalic  acid.  Decomp.  by 
alkalies +Aq.  (Miller  and  Mathews,  J.  Am. 
Chem.  Soc.  1900,  22.  64.) 


COBALTIMOLYBDATE,  BARIUM  COBALTOUS 


28- 


Mercuric  cobalticyanide,  Hg3[Co(CN)6]2. . 

81.  sol.  in  H2O,  decomp.  by  boiling. 

Insol.  in  alcohol  and  ether.  Not  attacked 
by  HC1.  (Soenderop,  Dissert,  1899.) 

Mercuric    potassium    cobalticyanide, 
K6HgCo2(CN)14. 

Sol.  in  H2O  with  decomp.  Insol.  in  al- 
cohol. 81.  sol.  in  ether.  (Soenderop,  Dissert, 
1899.) 

K6Hg3Co4(CN)24.  (Soenderop,  Dissert. 
1899.) 

Mercuric  sodium  cobalticyanide, 

Na6Hg3Co4(CN)24+4H20. 
Extremely    deliquescent.      (Soenderop, 
Dissert,  1899. 

Nickel    cobalticyanide,     Ni3[Co(CN)6]2  + 

12H2O. 

Insol.  in  H2O  and  acids.  Not  attacked  by 
boiling  HCl+Aq.  Sol.  in  NH4OH+Aq. 
Decomp.  by  KOH+Aq. 

Nickel  cobalticyanide  ammonia, 

Ni3[Co(CN)r,]2,  4NH3+7H20. 
Insol.  in  H2O. 

Potassium   cobalticyanide,   K3Co(CN)e. 
Easily  sol.  in  H2O.    Insol.  in  alcohol. 

Potassium  strontium  cobalticyanide, 

KSrCo(CN)6+9H2O. 
Sol.  in  H2O.     (Weselsky.) 

Potassium  thallium  cobalticyanide, 

K3Tl3[Co(CN)6]2. 

More  sol.  in  H2O  than  corresponding 
K  salt.  (Fischer  and  Benzian,  Ch.  Z.  1902, 
26.  49.) 

Potassium  zinc  cobalticyanide, 

KZnCo(CN)6+3H2O. 
(Fischer  and  Cuntze,  Ch.  Z.  1902,  26.  873.) 

Potassium  cobalticyanide  mercuric  chloride, 

2K3Co(CN)6,  3HgCl2. 
(Soenderop,  Dissert.  1899.) 

Potassium    cobalticyanide    mercuric    iodide, 

4K3Co(CN)6,  HgI2. 

Sol.    in    H2O    with    subsequent    decomp. 

Sol.   in  alcohol  and  ether  with  decomp. 

(Soenderop,  Dissert,  1899.) 

Silver  cobalticyanide,  Ag3Co(CN)6. 

Insol.  in  H2O  and  acids.  Sol.  in  NH4OH  + 
Aq. 

Silver  cobalticyanide  ammonia,  Ag3Co(CN)6, 

NH3  +  ^H20. 
Insol.  in  H2O.    (Zwenger.) 


Sodium  cobalticyanide,  Na3Co(CN)6+2H2O. 
Easily  sol.  in  H2O;  insol.  in  alcohol. 

Sodium  zinc  cobalticyanide,   NaZnCo(CN)6 

+H20. 
(Fischer  and  Cuntze,  Ch.  Z.  1902,  26.  873.) 

Strontium    cobalticyanide,    Sr3[Co(CN)6]2  + 

10H2O. 
Very  sol.  in  H2O.    (Weselsky.) 

Thallium    cobalticyanide,    Tl3Co(CN)6. 

100  pts.  H2O  dissolve  3.6  pts.  at  0°,  5.86  pts. 
at  9.5°,  10.04  pts.  at  19.5°.  (Fronmuller,  B. 
11.  91.) 

Yttrium    cobalticyanide,    YCo(CN)6+2H2O 
Nearly  insol.  in  H2O.     (Cleve.) 

Zinc  cobalticyanide,  Zn3[Co(CN)6]2+12H2O. 
Sol.  in  HCl+Aq  and  salt  is  pptd.  by  dilu- 
tion with  H2O.  Decomp.  by  H2SO4.  Insol. 
in  K4Co(CN)6+Aq.  Sol.  in  NH4OH  and 
NH4Cl+Aq.  (Fischer  and  Cuntze,  Ch.  Z. 
1902,  26.  873.) 

Zinc    cobalticyanide    ammonia, 
Zn3[Co(CN)6]2,  5NH3. 

Decomp.  by  H2O  and  acids.  (Fischer  and 
Cuntze,  Ch.  Z.  1902,  26.  873.) 

Zn3[Co(CN)6]2,  6NH3.  (Fischer  and 
Cuntze.) 

+3H2O.    (Fischer  and  Cuntze.) 

Zn3[Co(CN)6]2,  10NH3+9H20.  Decomp. 
by  H2O.  (Fischer  and  Cuntze.) 

Cobaltimolybdic  acid. 

Ammonium  barium  cobaltous  cobaltimolyb- 
date, i^(NH4)2O,  l^BaO,  CoO,  CoO2, 

.   10MoO3+18^H2O. 

Difficultly  sol.  in  H2O.  (PYiedheim  and 
Keller,  B.  1906,  39.  4306.) 

Ammonium  cobaltous  cobaltimolybdate, 

2(NH4)20,  CoO,  Co02, 10Mo03+12H20. 

Much  more  sol.  in  H2O  than  3(NH4)2O, 

CoO,   Co02,    12MoO3+20H2O.     Sp.   gr.   of 

cold  sat.  solution  =  1.096.     (Friedheim  and 

K3(NH4)20,  CoO,  Co02,  12MoOs+20H20. 

100  cc.  cold  sat.  aqueous  solution  contain 
3  g.  of  the  salt.  Sp.gr.  of  the  solution  =  1.0234. 

Sol.  in  cone.  HC1. 

Decomp.  by  cone.  H2SO4,  by  KOH+Aq 
and  by  NaOH  +  Aq.  (Friedheim  and  Keller.) 

Barium    cobaltous    cobaltimolybdate, 

3BaO,  CoO,  CoO2,  9MoO3+25H2O. 
SI.  sol.  in  H2O.    (Friedheim  and  Keller.) 


288 


COBALTIMOLYBDATE,  COBALTOUS  POTASSIUM 


Cobaltous   potassium  cobaltimolybdate, 

CoO,    3K2O,    CoO2,    10MoO3+10H20. 
(Kurnakoff,  Ch.  Z.  1890,  14.  113.) 

+  11H2O.  Sol.  in  cone.  HC1.  Decomp.  by 
KOH+Aq  and  by  NaOH+Aq.  (Friedheim 
and  Keller.) 

3K2O,  CoO,  CoO2,  12MoO3+15H2O.  SI. 
sol.  in  H2O.  Sol.  in  cone.  HC1.  Decomp.  by 
KOH+Aq  and  by  NaOH+Aq.  (Friedheim 
and  Keller.) 

+20H2O.  (Kurnakoff,  Ch.  Z.  1890,  14. 
113.) 

Potassium  cobaltimolybdate, 
3K20,  CoO2,  9MoOi+ 
Ppt.     (Hall,  J.  Am.  Chem.  Soc.  1907,  29. 

Cobaltinitrocyanhydric  acid. 

Potassium   cobaltinitrocyanide, 

K4Co2rCN)9NO2+3H2O. 
Very  sol.   in   H2O   but   quickly   decomp. 
Insol.  in  alcohol.     (Rosenheim  and  Kop- 
pel,  Z.  anorg.  1898,  17.  68.) 

Silver  cobaltinitrocyanide, 
Co2Ag6NO2(CN)10+6H2O,  and  +21H2O. 
(Rosenheim  and  Koppel.) 

Sodium    cobaltinitrocyanide 


. 

Very  deliquescent.  Sol.  in  H2O.  (Rosen- 
heim and  Koppel.) 

Cobaltisulphurous  acid,  H6Co2(S03)6. 

Not  obtained  in  a  solid  state.  (Berglund, 
Acta  Lund.  1872.) 

Cobaltisulphites. 

The  cobaltisulphites  are  insol.  or  at  least 
very  si.  sol.  in  H2O.  (Berglund,  Acta  Lund. 
1872.  23.) 

Ammonium  cobaltous  cobaltisulphite, 

(NH4)2SO3,  2CoSO3,  Co2(SO3)3+14H2O  = 
(NH4)2Co2Co2(SO3)6+14H2O. 

Scarcely  sol.  in  H2O,  but  decomp.  thereby. 

Easily  sol.  in  acids,  when  finely  divided; 
also  in  H2SO3  +Aq.  (Berglund.) 

2(NH4)2S03,    CoS03,    Co«(S03)3+8H20  = 
(NH4)4CoCo2(SO3)6+8H2O.      As    above. 
CBerglund.) 

Barium  cobaltisulphite.  3BaSO3,  Co2(SO3)8  + 

12H20=Ba3Co2(S03)6+12H20. 
Ppt.    Insol.  in  H2O,    Not  attacked  by  cold 
acids  even  H2SO4,  but  is  decomp.  by  boiling 
therewirth.    (Berglund,  Acta  Lund.  1872.) 

Bismuth    cobaltisulphite,    Bi2Co2(SO3)6. 

Insol.  in  H2O,  dil.  HNO3,  or  HCl+Aq. 
(Berglund,  Acta  Lund.  1872.  31.) 


Calcium  cobaltisulphite,  Ca3Co2(SO)3)6. 

Ppt.  Insol.  in  H2O  or  HCl+Aq.  (Berg- 
lund, Acta  Lund.  1872.  30.) 

Cobaltous     cobaltisulphite,     Co3Coo(SO3)6  = 

3CoS03,   Co2(S03)3. 
Ppt.    (Berglund,  B.  7.  470.) 

Cobaltous   potassium   cobaltisulphite, 

CoK4Co2(S03)6. 
Insol.  in  H2O.    (Berglund.) 

Silver  cobaltisulphite,   Co2(SO3)3,   3Ag2SO3. 
Properties  as  the  following  comp.     (Berg- 
lund.) 

Silver    cobaltous    cobaltisulphite,    CoSO3, 

Co2(SO3)3,    2Ag2SO3+9H2O. 
Insol.  in  H2O.    Insol.  in  HNO3+Aq.    De- 
comp. by  HC1  or  H2S+Aq.    (Berglund.) 

Sodium  cobaltous  cobaltisulphite. 

Decomp.  by  H2O,  so  that  it  has  not  been 
obtained  pure.  (Berglund,  Acta  Lund.  1872, 
29.) 

Cobaltoctamine  sulphurous  acid. 
See  Octamine  cobaltisulphurous  acid. 

Cobaltocobalticyanhydric  acid, 

H3Co3(CN)n. 

Unstable.  (Jackson  and  Comey,  Am.  Ch. 
J.  1897.  19,  277.) 

Barium   cobaltocobalticyanide, 

BaHCos(CN)n+l^H2O. 
Somewhat  sol.  in  H2O  when  pure. 
The  crude  salt  is  insol.  even  in  hot  H2O. 
(Jackson  and  Comey.) 

Cupric  cobaltocobalticyanide,   Cu3Co6(CN)22 
+4H2O. 

Ppt.    (Jackson  and  Comey.) 

Potassium   hydrogen    cobaltocobalticyanide. 

K2HCo3(CN)H+2H20. 

SI.  sol.  in  cold,  easily  sol.  in  hot  H2O. 

Insol.  in  alcohol.    (Jackson  and  Comey.) 

KH2Co3(CN)u+H2O.  Insol.  in  cold  or 
hot  H2O  when  impure. 

The  pure  salt  is  slowly  sol.  in  cold  H2O. 

More  sol.  in  warm  H20.  (Jackson  and 
Comey.) 

Silver   cobaltocobalticyanide,    Ag3Co8(CN)u 
+H2O. 

Ppt.     (Jackson  and  Comey,  B.  1896,  29. 


Zinc    cobaltocobalticyanide, 
+3H20. 


ZnHCo3(CN)n 


Ppfc.    (Jackson  and  Comey.) 


COLUMBATE,  MANGANOUS 


289 


Cobaltocyanhydric  acid,  H4Co(CN)6. 

Very  unstable.  Sol.  in  H2O.  Insol.  in 
alcohol. 

Cuprous  potassium  cobaltocyanide, 

K3CuCo(CN)6. 
(Straus,  Z.  anorg.  1895,  9.  17.) 

Potassium  cobaltocyanide,  K4Co(CN)6. 

Decomp.  on  air.  Very  deliquescent,  and 
sol.  in  H2O.  Insol.  in  alcohol  and  ether 
(Descamps,  Zeit.  Ch.  1868.  952.) 

Cobaltous  acid. 

Barium  cobaltite,  BaCo03. 

Insol.  in  H2O  or  dil.  HC2H302+Aq.    Sol 
in  HCl+Aq.    (Rousseau,  C.  R.  109.  64.) 

BaCo2Os.    As  above.    (Rousseau.) 

Cobaltous  potassium  cobaltite,  3Co02,  CoO, 


Rapidly  hydrolysed  by  H2O. 
Sol.  in  cone.  HC1.     (Bellucci,  Chem.  Soc 
1907,  92,  (2)  354.) 

Magnesium  cobaltite,  MgCo03. 

Insol.  in  H2O,  NH4OH,  or  (NH4)2CO3+Aq. 
Easily  sol.  in  NH4Cl+Aq,  from  which  it  is 
pptd.  by  KOH+Aq.  (Berzelius,  Pogg.  33. 
126.) 

Sol.  in  HF,  HC1,  HNO3+H2S04;  decomp. 
and  partially  dissolved  by  NH4OH+Aq;  quite 
stable  when  heated.  (Dufau,  C.  R.  1896, 
123.  240.) 

Potassium  cobaltite. 

According  to  Bellucci  and  Dominici  the 
compounds  formerly  described  are  more  or 
less  decomp.  by  hydrolysis.  (C.  C.  1907. 
I,  1530.) 

Sodium  cobaltite. 

Sol.  in  NaOH+Aq,  but  pptd.  by  diluting 
the  solution. 

Columbic  acid  (Niobic  acid),  3Cb2O6, 
4H2O,  or  3Cb206,  7H2O. 

Easily  sol.  in  HF;  very  si.  sol.  in  HCl+Aq, 
but  is  sol.  in  H2O  after  being  treated  with 
HCl+Aq.  Sol.  in  cone.  H2S04.  Sol.  in 
KOH+Aq.  Insol.  in  NaOH+Aq,  but  be- 
comes sol.  in  H2O  by  being  treated  with 
NaOH+Aq.  Sol,  in  boiling  Na2CO3+Aq. 
(Rose,  Pogg.  113.  109.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  830.) 

Cb2O5,  4HoO. 

Cb205,  7H2O.  (Santesson,  Bull.  Soc.  (2) 
24.  52.) 

Aluminum  columbate,  A12OS,  3Cb2O6+12H2O. 
Ppt.     (E.  F.  Smith,  J.  Am.  Chem.  Soc. 
1908,  30.  1652.) 


Barium  columbate,  7BaO,  6Cb2O6+18H2O. 
Ppt.     (Bedford,  J.  Am.  Chem.  Soc.  1905, 
27.  1218.) 

Cadmium  columbate,  CdO,  Cb2O6. 

Sol.  in  boiling  cone.  H2SO4;  insol.  in  most 
acids;  decomp.  by  HKS04  at  red  heat.  (Lars- 
son,  Z.  anorg.  1896,  12.  199.) 

+3^H2O,  Ppt.  (E.  F.  Smith,  J.  Am. 
Chem.  Soc.  1908,  30.  1652.) 

Caesium  columbate,  4Cs2O,  3Cb2O6+14H20. 

Very  sol.  in  H2O.  (E.  F.  Smith,  J.  Am. 
Chem.  Soc.  1908,  30.  1654.) 

7Cs2O,  6Cb2O6+30H20.  Ppt.  (E.  F. 
Smith,  J.  Am.  Chem.  Soc.  1908,  30.  1655.) 

Calcium  columbate,  2CaO,  Cb2O5. 
Insol.  in  H2O.    (Joly,  C.  R.  81.  266.) 
CaO,  Cb2O5.    Sol.  in  boiling  cone.  H2SO4; 
insol.  in  most  acids;  decomp.  by  HKSO4  at 
red  heat.    (Larsson,  Z.  anorg.  1896,  12.  198.) 

Cobalt  columbate,  CoO,  Cb206. 

Sol.  in  cone,  boiling  H2SO4;  insol.  in  most 
acids;  decomp.  by  HKSO4  at  red  heat.  (Lars- 
son.) 

Copper  columbate,  CuO,  Cb2O6. 

Sol.  in  boiling  cone.  H2SO4;  insol.  in  most 
acids;  decomp.  by  HKSO4  at  red  heat.  (Lars- 
son.) 

+3^H2O.  Ppt.  (E.  F.  Smith,  J.  Am. 
Chem.  Soc.  1908,  30.  1652.) 

Iron  (ferrous)  columbate,  Fe(CbO3)2. 
Min.  Columbite.    Insol.  in  acids. 

Iron  (ferrous)  columbate  tantalate, 

zFe(TaO8)2, 2/Fe(CbO3)2. 
Min.   Tantalite.     Not  attacked  by  acids. 
Fe(Cb03)2,   4Fe(TaO,)2.     Min.    Tapiolite. 

Lithium  columbate,  7Li2O,  6Cb2O6+26H2O. 
Ppt.  (E.  F.  Smith,  J.  Am.  Chem.  Soc. 
1908,  30.  1655.) 

Magnesium  columbate,  MgO,  Cb2O6. 

Sol.  in  boiling  cone.  H2SO4;  insol.  in  most 
acids;  decomp.  by  KHSO4  at  red  heat.  (Lars- 
son,  Z.  anorg.  1896, 12. 196.) 

+4H2O.    Precipitate.    (Rammelsberg.) 

+7H2O.  Ppt.  (E.  F.  Smith,  J.  Am. 
ihem.  Soc.  1908,  30.  1651.) 

4MgO,  Cb2O8.  Insol.  in  H2O.  (Joly,  C.  R. 
81.  266.) 

3MgO,  Cb206.    As  above. 

Manganous  columbate. 
Insol.  in  H2O.    (Joly,  C.  R.  81.  266.) 
3MnO,  5Cb2O6.  Sol.  in  boiling  cone.  H2SO4; 
nsol.  in  most  acids;  decomp.  by  HKSO4  at 
red  heat.    (Larsson,  Z.  anorg.  1896,  12.  201.) 


290 


COLUMBATE,  POTASSIUM 


Potassium  columbate,  KCbO*. 

Sol.  in  H2O.    (Joly,  in  Fremy's  Encyc.  Ch.) 

K2Cb4O7+5^H2O.  Insol.  in  H2O.  (San- 
tesson.) 

K2Cb6O16+5H2O.    Nearly  insol.  in  H2O. 

K4Cb2O7+llH2O.  Insol.  in  H2O.  (San- 
tesson,  Bull.  Soc.  (2)  24.  53.) 

K4Cb8O22+HH2O.     (Santesson.) 

K6Cb4013+13H2O.    Sol.  in  H2O. 

K8Cb6Oio+16H20.  Efflorescent.  Sol.  in 
H2O.  (Marignac,  A.  ch.  (4)  8.  20.) 

Very  sol.  in  H2O.  (E.  F.  Smith,  J.  Am. 
Chem.  Soc.  1908,  30.  1652.) 

K14Cb12O37+27H2O.  Sol.  in  H2O.  Insol. 
in  alcohol.  (E.  F.  Smith.) 

K16Cb14O«+32H2O.    Sol.  in  H2O. 

Potassium  sodium  columbate,  3K2O,  Na2O, 

3Cb2O6+9H2O. 

Very  slightly  sol.  in  H2O.  Insol.  in  alkalies. 
(Marignac.) 

Rubidium  columbate,  3Rb2O,  4Cb2O6+ 


(E.  F.  Smith,  J.  Am.  Chem.  Soc.  1908,  30. 
1655.) 

4Rb20.3Cb2O6+14H2O.  Very  sol.  in  H2O. 
(E.  F.  Smith.) 

Silver  columbate,  Ag20,  Cb2O6+2H2O. 

Ppt.    (E.  F.  Smith.) 

7Ag2O,  6Cb2O6+5H2O.  Insol.  in  H2O. 
(Bedford,  J.  Am.  Chem.  Soc.  1905,  27.  1218.) 

Sodium  columbate,   NaCbO3+3^H2O. 

Completely  sol.  in  H2O.    (Rose). 

Ppt.  (E.  F.  Smith,  J.  Am.  Chem.  Soc.  1908, 
30.  1651.) 

+2^H2O.  SI.  sol.  in  cold  H2O.  Insol.  in 
JSTaOH+Aq.  (Santesson.) 

2Na2O,  3Cb2O6+9H20.  Insol.  in  H20  or 
.NaOH+Aq.  (Santesson.) 

8Na2O,  7Cb2O6.  1  pt.  is  sol.  in  195-200  pts. 
H2O  at  14-20°;  in  ether  75-80  pts.  or  in  103 
pts.  boiling  water.  (Rose.) 

7Na2O,  6Cb2O5+32H2O.     Very  stable. 

Sol.  in  H2O.  (Bedford,  J.  Am.  Chem.  Soc. 
1905,  27.  1217.) 

Thorium  columbate,  5Th2O,  16Cb2O6. 

Sol.  in  boiling  cone.  H2SO4;  insol.  in  most 
-acids;  decomp.  by  HKSO4  at  red  heat.  (Lars- 
son,  Z.  anorg.  1896,  12.  202.) 

Yttrium  columbate,  Y2O3,  Cb2O5. 
Insol.  in  H2O.    (Joly,  C.  R.  81.  1261.) 
Sol.  in  boiling  cone.  H2SO4;  insol.  in  most 

acids;  decomp.  by  HKS04  at  red  heat.    (Lars- 

son.) 

Zinc  columbate,  ZnO,  Cb2O,. 

Sol.  in  boiling  cone.  H2SO4;  insol.  in  most 
acids;  decomp.  by  HKSO4  at  red  heat.  (Lars- 
son.) 


7ZnO,  6Cb2O6+25H2O.    Insol.  in  H2O. 
(Bedford,  J.  Am.  Chem.  Soc.  1905,  27.  1218.) 

Zirconium  columbate,  ZrO2,  5Cb2O5. 

Sol.  in  boiling  cone.  H2SO4;  insol.  in  most 
acids;  decomp.  by  HKSO4  at  red  heat.  (Lars- 
son.) 

Percolumbic  acid. 
See  Percolumbic  acid. 

Columbium  (Niobium),  Cb. 

Scarcely  attacked  by  HC1,  HNO3,  or  aqua 
regia.  Cone.  H2S04  dissolves  easily  on  warm- 
ing. 

Sol.  in  fused  oxidizing  agents;  sol.  in  hot 
cone.  H2SO4  and  in  HF;  also  in  HF+HNO3; 
insol.  in  other  acids.  (Moissan,  C.  R.  1901, 
133.  24.) 

Columbium  pentabromide,  CbCr5. 
(Rose,  Pogg.  104.  422.) 

Columbium  carbide  nitride,  3CbC,  2CbN. 
(Joly,  Bull.  Soc.  (2)  25.  506.) 

Columbium  trichloride,  CbCl3. 

Not  deliquescent;  not  attacked  by  H2O, 
but  easily  oxidised  by  HNO3+Aq.  Insol.  in 
NH4OH+Aq.  (Roscoe,  C.  N.  37.  25.) 

Columbium  pentochloride,  CbCl6. 

Decomp.  by  H2O  with  separation  of  a 
hydrate  of  Cb2O6.  Sol.  in  cold  HCl+Aq, 
forming  a  solution  which  soon  gelatinises,  and 
separates  out'Cb2O6  by  heat  or  dilution;  with 
hot  HCl+Aq,  forms  a  cloudy  solution  which 
does  not  gelatinise.  Sol.^  in  H2SO4  to  form  a 
clear  liquid  which  gelatinises  on  heating.  Sol. 
in  KOH+Aq.  Sol.  in  alcohol  with  slight 
residue.  (Rose,  Pogg.  104.  432.) 

Columbium  pentafluoride,  CbFB. 

Very  hydroscopic;  sol.  in  H2O  without 
separation  of  columbic  acid.  (Ruff,  B.  1909, 
42.  492.) 

Columbium  fluoride  with  MF. 
See  Fluocolumbate,  M. 

Columbium  hydride,  CbH(?). 

Insol.  in  HC1,  HNO?,  and  dil.  H2SO4+Aq, 
even  on  boiling.  Sol.  in  boiling  cone.  H2SO4 
and  in  fused  KHS04.  Sol.  in  cold  HF+Aq 
if  not  too  dilute.  Also  attacked  by  KOH  + 
Aq.  (Marignac,  N.  Arch.  Phys.  Nat.  31.  89.) 

Not  attacked  by  boiling  H2O,  or  boiling 
HC1. 

Oxidized  by  hot  H2SO4.  Insol.  in  boiling 
HNO3.  (Muthmann,  A.  1907,  355.  90.) 

Columbium  hydroxide  Cb205,  zH20. 
See  Columbic  acid. 


COPPER 


291 


Columbium  nitride. 

Not  attacked  by  boiling  nitric  acid  or  aqua 
regia,  but  sol.  in  a  cold  mixture  of  HNO3  and 
HF.  (Rose,  Pogg.  111.  426.) 

Cb3NB.  Not  attacked  by  boiling  H2O  or 
HC1.  Insol.  in  cone.  HNO3,  and  H2SO4. 

Decomp.  by  fused  KOH.  Not  attacked  by 
boiling  with  KOH+Aq.  (Muthmann,  A. 
1907,  356.  94.) 

Columbium  dioxide,  Cb2O2. 

Sol.  when  still  moist  in  boiling  dil.  HC1  + 
Aq.  Insol.  in  hot  HNO3;  less  sol.  in  aqua 
regia  than  in  HCl+Aq.  Sol.  in  cone.  H2SO4 
after  long  heating.  (Rose.) 

Insol.  in  H2O,  KOH,  or  cone,  acids,  even 
when  boiling.  (Delafontaine.) 

Columbium  Zn'oxide,  Cb2O3. 

Insol.  in  acids  except  HF.  (Smith,  Z. 
anorg.  1894,  7. 28.) 

Columbium  tetroxide,  Cb2O4. 

Not  attacked  by  cold  or  hot  H2O,  HC1, 
HNO3,  H2SO4,  9r  aqua  regia.  Slightly  at- 
tacked by  boiling  KOH+Aq.  (Delafon- 
taine.) 

Columbium  pentoxide,  Cb2O5. 

When  ignited  insol.  in  hot  cone.  H2S04. 
When  it  has  not  been  ignited  it  forms  a  clear 
solution  with  H2SO4,  which  can  be  diluted 
without  forming  any  precipitate.  (Rose, 
Pogg.  112.  549.) 

Sol.  in  fused  KHSO4,  which  can  be  diluted 
with  H2O  without  causing  pptn.  Insol.  in 
HF. 

Columbium  oxybromide,  CbOBr3. 

Decomp.  by  H2O  into  Cb2O5  and  HBr.  Sol. 
in  hot  H2SO4  and  cone.  HCl+Aq.  (Rose, 
Pogg.  104.  442.) 

3H2O,  Cb2O4,  HBr(?).  Easily  sublimed. 
(Smith,  Z.  anorg.  1894,  7.  97.) 

Columbium  oxybromide  rubidium  bromide, 

CbOBr3,  2RbBr. 

Unstable  in  moist  air.  Decomp.  by  H2O. 
(Weinland,  B.  1905,  39.  3059.) 

Columbium  oxychloride,  CbOCl3. 

Attracts  H2O  from  air  without  deliquescing 
and  decomposed.  Decomp.  with  H2O  with 
evolution  of  heat.  Insol.  in  hot  or  cold  HC1+ 
Aq.  Sol.  by  long  contact  with  H2SO4  to  a 
cloudy  liquid,  which  clears  up  on  warming, 
but  soon  separates  out  Cb2O5.  Sol.  in  cold 
KOH+Aq  and  hot  K2CO3+Aq.  /Rose.) 

Sol.  in  alcohol,  from  which  it  is  precipitated 
by  ether.  (Blomstrand.) 

3H2O,  Cb2O4,  HC1.  Sublimate.  (Smith, 
Z.  anorg.  1894,  7.  97.) 

Columbium  oxychloride  rubidium  chloride, 

CbOCl3,  2RbCl. 

Decomp.  by  H2O.  (Weinland,  B.  1906, 
39.  3057.) 


Columbium  oxyfluoride,  CbOF3. 
(Joly,  C.  R.  81.  1266.) 

Columbium  oxyfluoride  with  MF. 

See  Fluoxycolumbate,  and  Fluoxyhypo- 
columbate,  M. 

Columbium  oxysulphide,  Cb2OS8. 

Insol.  in  boiling  HCl+Aq.  Slowly  decomp. 
into  Cb2O6  by  boiling  with  HNO3  or  aqua 
regia.  Insol.  in  boiling  dil.  H2SO4+Aq. 
Converted  into  columbic  sulphate,  sol.  in  H2O, 
by  boiling  cone.  H2SO4.  SI.  sol.  in  hot  HF. 
Insol.  in  boiling  K2S+Aq.  (Rose,  Pogg.  111. 

193.) 

- 

Copper,  Cu. 

Copper  is  not  attacked  by  distilled  H2O,  or 
by  NH4NO3,  KNO3,  or  (NH4)2SO4+Aq,  or  by 
a  mixture  of  those  salts  in  solution.  (Muir, 
cited  by  Carnelly,  Chem.  Soc.  30.  1.) 

Distilled  H2O  has  slight  action  on  Cu.  100 
ccm.  H2O  dissolved  from  2  sq.  dcm.  Cu  from 
0.035  mg.  Cu  in  one  hour  up  to  0.280  mg.  in 
72  hours.  100  ccm.  H2O  dissolved  0.44  mg. 
from  6  sq.  dcm.  in  48  hours.  Presence  of 
solder  diminishes  solubility  about  one-half. 
At  90-100°  the  amount  dissolved  is  about  one- 
half  that  at  ord.  temp.  (Carnelley,  Chem. 
Soc.  30.  1.) 

100  ccm.  distilled  H2O  dissolved  only  1 
mg.  Cu  from  11.8  sq.  cm.  during  a  week,  while 
air  free  from  CO2  was  conducted  through  the 
solution.  When  the  air  contained  CO2l  3  mg. 
were  dissolved.  (Wagner,  Dingl.  221.  259.) 

100  1.  sea  water  dissolved  12.96  g.  Cu  from 
1  sq.  m.  (Calvert  and  Johnson,  C.  N.  11. 
171.) 

Solubility  in  H2SO4. 

Not  attacked  by  dil.  H2S04+Aq.  (Vogel, 
Schw.  J.  32.  301.) 

Action  of  H2SO4  at  ordinary  temp,  is  very 
slight  even  after  a  long  time.  (Barruel,  J. 
Pharm.  20.  13  [1834].) 

H2SO4  has  no  action  below  130°.  (Calverfc 
and  Johnson,  Chem.  Soc.  19.  438.) 

H2S04  acts  slightly  even  at  20.°   • 
16.3  g.  H2SO4  (1.843  sp.  gr.)  dissolved  the 
following  amts.  from  3  g.  Cu,  having  a 
surface  of  65  sq.  cm.  at  the  given  temp. 


Temp. 

Time 

%  Cu  dissolved 

19° 

14  days 

About  6 

60 

120  min. 

2.5 

80 

30 

1.5 

100 

30 

3.1 

124 

30 

22.7 

130 

30 

32.6 

137 

30 

35  0 

150 

30 

69.2 

170 

10 

51.92 

195 

2 

53.5 

220 

H 

70.57 

270 

few  seconds 

nearly  100 

292 


COPPER 


With  dilute  acid  the  action  was  much  less 
violent,  as  is  seen  in  the  following  table — 


Tern. 

Time 

Acid 

Sp.  gr. 

%Cu 
dissolved 

100° 

30  min. 

H2SO4 

1.843 

2.380 

100 

30 

2H2SO4,  H20 

.8295 

0.585 

100 

30 

H2SO4,  H2O 

.780 

0 

100 
130 

30 
30 

H2S04,  2H2O 
H2SO4 

.620 
.843 

0 
32.6 

130 

30 

H2S04,  H20 

.780 

1.18 

130 
165 

30 
15 

H2S04,  2H20 
H2SO4 

.620 
.843 

0 
70 

165 

30 

H2SO4,  H2O 

1.780 

16.5 

165 

30 

H2S04,  2H2O 

1.620 

2.7 

(Pickering,  Chem.  Soc.  33.  112.) 

Cu  is  very  si.  attacked  by  cold  HCl+Aq  of 
1.12  sp.  gr.,  but  somewhat  more  on  warming. 
Even  less  sol.  in  dil.  HCl+Aq.  (Lowe,  Z. 
anal.  4.  361.) 

Sol.  in  warm  cone.  HI+Aq.     (Rose.) 

Slowly  attacked  by  H2S03+Aq.  (Causse, 
Bull.  Soc.  (2)  46. 3.) 

More  or  less  sol.  in  all  dil.  mineral  acids  and 
also  in  organic  acids,  as  acetic,  tartaric,  etc., 
when  supply  of  air  is  afforded;  but  absolutely 
insol.  in  the  latter  acids  when  air  is  wholly 
excluded.  The  importance  of  this  fact  in  the 
use  of  Cu  cooking  utensils  is  manifest. 

Easily  attacked  by  ord.  HNO3+Aq. 

With  very  cone.  HN03+Aq  (sp.  gr.  1.52)  it 
becomes  passive,  as  in  the  case  of  Fe. 

Pure  dil.  HNO3+Aq  of  1.07  sp.  gr.  or  less 
does  not  attack  Cu  at  20°,  but  if  NO2  or 
KNO2,  is  added  the  action  begins  at  once.  If 
HNO3+Aq  is  more  cone,  the  Cu  is  attacked. 
HNO3+Aq  of  1.108  sp.  gr.  begins  to  act  at 
-2°,  and  of  1.217  sp.  gr.  at  -10°. 

HNOs+Aq  of  1.512  sp.  gr.  attacks  Cu  vio- 
lently at  20°,  but  action  soon  ceases  on  ac- 
count of  formation  of  a  crust  of  Cu(NO3)2, 
insol.  in  pure  HNO3.  (Millon,  A.  ch.  (3)  6. 
95.) 

Easily  sol.  in  2N-HClO3+Aq  at  50°. 
(Hendrixson,  J.  Am.  Chem.  Soc.  1904,  26. 
756.) 

Not  appreciably  sol.  in  anhydrous  HF. 
(Poulenc,  A.  ch.  1894,  (7)  2.  12.) 

When  in  contact  with  the  air,  Cu  is  soon 
oxidised  by  acids,  alkalies  (especially  NH4OH 
+Aq),  and  many  fatty  bodies. 

Sol.  in  (NH4y2CO3+Aq.  (Traube,  B.  18. 
1887.) 

Slowly  sol.  in  NH4OH+Aq.  (Schonbein, 
B.  A.  B.  1866.  580.) 

Sol.  in  KI+Aq  when  warm  and  cone. 
(Rose.) 

When  finely  divided,  Cu  is  easily  sol.  in  hot 
FeCl3+Aq. 


Action  of  dilute  solutions  of  salts  on  solubil- 
ity of  Cu  in  H2O. 

100  ccm.  solution  of  the  following  salts  dis- 
solve the  amts.  of  Cu  given  below,  from  a 
surface  of  1  sq.  dcm.  in  48  hours. 


Salts 

G.  salt  dissolved 
in  100  ccm.  HjO 

Mg.  Cu  dis- 
solved 

H2O 

0.11 

KN03 

0.01 
0.05 
5.00 

0.07 
0.13 
0.16 

NaN03       { 

0.05 
5.00 

0.18 
0.19 

CaS04 

0.05 

0.11 

K2S04        { 

0.05 
5.00 

0.12 
0.28 

MgSO4 

0.05 
5.00 

0.16 
0.34 

f 
Na2CO3 

i 

0.01 
0.05 
5.00 

0.05 
0.11 
2.80 

K2C03       { 

0.05 
5.00 

0.14 
2.35 

NaCl 

0.01 
0.05 
5.00 

0.05 
0.18 
7.50 

KC1 

5.00 

8.17 

(NH4)2S04    { 

0.05 
5.00 

0.66 
28.50 

NH4N08 

0.01 
0.05 
5.00 

0.17 
0.66 
60.00 

NH4C1       { 

0.05 
5.00 

0.92 
158.75 

At  100°  the  action  of  KN03,  K2SO4,  and 
NH4NO3  is  diminished,  while  that  of 
(NH4)2S04,  Na2C03?  and  NaCl  is  increased. 

Tables  are  also  given  for  mixtures  of  the 
above  salts.  (Carnelley,  Chem.  Soc.  30.  1.) 

Solubility  of  Cu  in  dilute  salt  solutions. 

11.8  sq.  cm.  Cu  were  used,  and  the  action 
continued  one  week,  while  air  with  or  without 
CO2  was  passed  through  the  solution  con- 
tinually. 


CUPROUS  ACETYLIDE  IODIDE 


293 


100  ccm.  solution  of  the  following  salts  dis- 
solved the  given  amts.    Cu. 


Salt 

G.  salt  dis- 
solved in 
100  ccm.  H2O 

Mg.  Cu  dis- 
solved with- 
out CO2 

Mg.  Cu 
dissolved 
with  CO2 

NaCl 
KC1 
MgCl2 
NH4C1 
K2S04 
KN03 
Na2C03 
NaOH 
CaO2H2 

0.50 
0.50 
0.83 
1.00 
1.00 
1.00 
1.00 
0.923 
sat. 

4 
4 
5 
904 
0 
0 
0 
0 
0 

115 
115 
112 
138 
4 
3 

(Wagner,  Dingl.  221.  260.) 

Distilled  H2O  dissolved  no  Cu  from  420  sq. 
mm.  in  150  hours  at  ord.  temp. 

NH4NO3+Aq  with  less  than  0.4  g.  per  litre 
showed  the  same  result. 

KNOs+Aq  or  (NH4)2SO4+Aq  contain- 
ing 0.1  to  0.2  g.  per  litre  dissolved  no  Cu. 

H2O  containing  carbonates +nitrates,  car- 
bonates +  sulphates,  or  chlorides  -f  nitrates 
also  dissolved  no  Cu. 

NH4NO3+Aq  containing  0.4  g.  per  litre 
dissolved  3  mg.  per  litre  after  150  hours 
contact. 

From  a  surface  of  2100  sq.  m.  of  Cu,  H2O 
charged  with  C02  at  ord.  pressure,  and  con- 
taining the  following  salts  in  solution,  dis- 
solved the  given  amts.  Cu.  in  120  hours. 


Salt 

G.  salt  dissolved 
in  1  1.  H20 

Mg.  Cu 
dissolved 

H2O 

1.0 

K2C03 

Q.2 

0.2 

CaCl2 

0.2 

1.80 

NH4N03 

0.02 

1.40 

NH4NO3 

0.04 

1.40 

K2C03  +     { 

0.1     ) 

NH4NO3       1 

0.02 

1.00 

K2C03  + 

0.2 

NH4NO3       1 

0.04 

0.1 

NH4N03+   j 

0.2 

CaCl2         ( 

0.2 

3.6 

From  a  surface  of  2100  sq.  m.,  H2O  charged 
with  CO2  at  pressure  of  6  atmos.  dissolved  0.6 
mg.  in  48  hours. 

H2O  when  charged  with  CO2  at  6  atmos.  and 
containing: 

16  mg.  NH4NO3  per  litre,  dissolved  0.8  mg. 
in  48  hours. 

•  80  mg.  NH4NO3  per  litre,  dissolved   1.4 
mg.  in  48  hours. 

40  mg.  K2CO3,  per  litre,  dissolved  1.2  mg 
in  48  hours.  (Muir,  Proc.  Soc.  Manchester, 
15.  31.) 

Sol.  in  KCN+Aq.  (Goyder,  C.  N.  1894, 
69.  262.) 

A  solution  of  (NH4)2S208  containing  0.829  g. 


in    110   cc.   dissolves   0.2050-0.2279  g.   Cu. 
(Turrentine,  J.  phys.  Chem.  1907,  11.  625.) 

SI.  attacked  by  liquid  NH3.     (Franklin, 
Am.  Ch.  J.  1898,  20.  827.) 

Amts.  Cu  dissolved  by  action  of  various  oils 
on  8  sq.  in.  Cu  by  10  days'  exposure  and 
subsequent  67  days — • 


Linseed  oil  . 
Olive  oil  ".  . 
Colza  oil .  . 
Almond  oil  . 
Seal  oil  .  . 
Sperm  oil 
Castor  oil  . 
Neatsfoot  oil 
Sesame  oil  . 
Paraffine  oil . 


Amt.  Cu  dis- 
solved in  10  days 

Amt.  Cu  dissolved 
•in  subsequent  67 
days 

0.3000  grain 

0.2435  grain 

0.2200 

0.0200      " 

0.0170 

0.1230      " 

0.1030 

0.1170      " 

0.0485 

0.0315       " 

0.0030 

0.0575       " 

0.0065 

0.0035      " 

0.1100 

.... 

0.1700 

o.oois"  " 

0.0015     " 

(Watson,  C.  N.  36.  200.) 

Qualitative  results  of  the  action  of  various 
oils  on  Cu  are  also  given  by  Thompson. 
(C.  N.  34. 176,  200,  219.) 

%  ccm.  oleic  acid  dissolves  0.0157  g.  Cu 
in  6  days.  (Gates,  J.  phys.  Chem.  1911, 
15.  143.) 

Sol.  in  an  alkaline  solution  of  gelatine  (3.54 
%)  copper  gauze  dissolved  in  48  hours. 
(Lidoff,  C.  C.  1899,  II.  471.) 

Cuprous  acetylide,  Cu2C2. 

Decomp.  by  heating  with  H2O  or  KCN-f 
Aq.  Decomp.  by  HNO3.  (Keiser,  Am.  Ch. 
J.  1892,  14.  289.) 

Not  decomp.  by  H2SO4,  NH4OH,  KOH  + 
Aq  or  acetic  acid,  even  on  warming.  The 
dry  salt  is  sol.  in  very  dil.  HCl+Aq  without 
evolution  of  gas.  Sol.  in  cone.  KCN+Aq. 
(Bottger,  A.  1859,  109.  356.) 

Cupric  acetylide,  CuC2. 

Easily  sol.  in  HC1.  Turns  brown  in  the  air, 
and  becomes  insol.  in  acids.  (Phillips,  Z. 
anorg.  1894,  6.  241.) 

3Cu4C8O+2H2O.  Solubility  as  that  of 
Cu8CnH4O3.  (Soderbaum,  B.  1897,  30.  764.) 

Cu8Ci7H4O3.    Insol.  in  H2O. 

When  dry  is  violently  decomp.  by  cone. 
H2S04  or  not  too  dil.  HNO3.  Rapidly  de- 
comp. by  warming  with  dil.  acids,  especially 
HC1. 

Insol.  in  NH4OH+Aq  in  absence  of  air, 
partially  sol.  in  presence  of  air. 

Insol.  in  organic  solvents.  (Soderbaum, 
B.  1897,  30.  762.) 

Cuprous  acetylide  iodide,  Cu3C2I,  Cul. 

Ppt.  (Berthelot  and  Delepine,  A.  ch. 
1900,  (7)  19.  54.) 


294 


CUPRIC  ARSENIDE 


Cupric  arsenide,  Cu6As2. 

(Reinsch,  J.  pr.  24.  244.) 

Cu4As2.    (Gehlen.) 

Cu3As2.  Ppt.  Decomp.  by  acids.  (Kane, 
Pogg.  44.  471.) 

Cu3As.  Min.  Domeykite.  Insol.  in  HC1 
+Aq;  sol.  in  HNO3. 

Cu6As.     Min.  Algodonite. 

Cu9As.     Min.  Darwinite. 

Cuprous  azoimide,  CuN3. 

Insol.  in  H2O.     (Curtius.) 

Sensitive  to  sunlight.  (Wohler,  B.  1913, 
46.  2053.) 

Cupric  azoimide,  basic,  CuO,  CuN6. 

Insol.  in  H2O.    (Wohler,  B.  1913,  46.  2055.) 

Cupric  azoimide,  CuN6. 

Very  explosive. 

Very  si.  sol.  in  H2O.  Decomp.  by  boiling 
with  H2O.  (Curtius,  J.  pr.  1898,  (2)  58. 
296.) 

Copper  azoimide  ammonia,  CuNs,  2NH3. 

Ppt.  Insol.  in  H2O.  Easily  sol.  in  dil. 
acids.  (Dennis,  J.  Am.  Chem.  Soc.  1907. 
29,  19.) 

Copper  boride,  Cu3B2. 

(Marsden,  J.  B.,  1880.  330.) 

Cuprous  bromide,  Cu2Br2. 

1  l.H2O  dissolves  at  18°-20°: 
0.4320  millimols  bromine. 
0.3157  cupric  copper. 

0.1061          "       cuprous  copper. 
(Bodlander,  Z.  anorg.  1902,  31.  460.) 

Sol.  in  HBr,  HC1  without  decomp.,  or 
HNO3+Aq  with  decomp.,  also  in  NH4OH 
+Aq.  Insol.  in  boiling  cone.  H2SO4  or 
HC2H3O2+Aq.  (Berthemot,  A.  ch.  44.  385.) 

Sol.  in  H2SO3+Aq.  (Lean  and  What- 
mough,  Chem.  Soc.  1898,  73.  151.) 

Sol.  in  NaCl,  and  Na2S2O3+Aq.  (Re- 
nault, C.  R.  69.  319.) 

Solubility  of  Cu2Br2  in  KBr+Aq. 
All  values  recorded  in  millimols  per  litre. 


KBr 

Total  copper 

Cupric 
copper 

Cuprous 
copper 

25 

0.119 

0.012 

0.107 

40 

0.200 

0.013 

0.187 

60 

0.310 

0.025 

0.285 

80 

0.423 

0.012 

0.411 

100 

0.5836 

.   0.5836 

120 

0.6934 

0.6934 

500 

8.719 

8.719 

(Bodlander  and  Storbeck,  Z.  anorg.  1902,  31. 
462.) 


Difficultly  sol.  in  methyl  acetate.  (Nau- 
mann,  B.  1909,  42.  3790.) 

Sol.  in  ethyl  acetate.    (Naumann,  B.  1910, 

43.  314.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329;  Eidmann,  C.  C.  1897,  II.  1014.) 

100  g.  acetonitrile  dissolve  3.86  g.  Cu2Br2 
at  18°.  (Naumann  and  Schier,  B.  1914,  47. 
249.) 

Sol.  in  pyridine.  (Naumann,  B.  1904,  37. 
4609.) 

Mol.  weight  determined  in  pyridine, 
methyl  and  ethyl  sulphides.  (Werner,  Z. 
anorg.  1897,  15.  19,  26,  and  28.) 

Cupric  bromide,  CuBr2. 

Deliquescent.  Very  sol.  in  H2O.  Insol.  in 
benzene.  (Franchimont,  B.  16.  387.) 

Very  si.  attacked  by  cold  or  even  hot 
H2S04.  (Viard,  C.  R.  1902,  135.  169.) 

Moderately  sol.  in  liquid  NH3.  (Horn, 
Am.  Ch.  J.  1908,  39.  219.) 

100  g.  95%  formic  acid  dissolve  0.16  g.  at 
21°.  (Aschan,  Ch.  Z.  1913,  37.  1117.) 

100  g.  acetonitrile  dissolve  24.43  g.  CuBr2 
at  18°.  (Naumann  and  Schier,  B.  1914,  47. 
249.) 

Sol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1369.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.)  . 

Sol.  in  acetone  with  a  brown  color.  (Eid- 
mann, C.  C.  1899,  II.  1014.) 

+2H2O(?).      (Berthemot,    A.    ch.    1830, 

44.  385.) 

+4H2O.  Very  sol.  in  H2O.  (Sabatier, 
Bull.  Soc.  1894,  (3)  11.  677.) 

Cupric  hydrogen  bromide,  CuBr2,  HBr+ 
2H2O. 

Decomp.  by  H20.  (Sabatier,  Bull.  Soc. 
1894,  (3)  11.  681.) 

+  10H2O.  (Weinland  and  Knoll,  Z.  anorg. 
1905,  44.  116.) 

Cupric  lithium  bromide,  CuBr2, 2LiBr +6H2O. 

Very  hydroscopic.  (Sementschenko,  Z. 
anorg.  1899,  19.  336.) 

Very  hydroscopic;  decomp.  by  H2O. 
(Kurnakoff,  C.  C.  1899,  I.  16.) 

Cupric  potassium  bromide,  CuBr2,  KBr. 

Decomp.  by  H2O.  (Sabatier,  Bull.  Soc. 
1894,  (3)  11.  683.) 

Cuprous  bromide  ammonia,  Cu2Br2,  2NH3. 

Stable  when  dry. 

Easily  sol.  in  HNO3  *and  NH4OH+Aq. 
Other  mineral  acids  and  acetic  acid  separate 
Cu2Br2.  (Richards,  Z.  anorg.  1898,  17.  245.) 

Cu2Br2,  6NH3.    (Lloyd.) 

Cu2Br2,  3NH3.  (Lloyd,  J.  phys.  Chem. 
1908,  12.  399.) 


CUPROUS  CHLORIDE 


295 


Cupric  bromide  ammonia,  CuBr2,  2NH3. 

Sol.  in  NH4Br+Aq  without  decomp. 
(Richards,  B.  23.  3790.) 

3CuBr2,  10NH3.  Decomp.  by  H2O. 
(Richards,  Am.  Ch.  J.  15.  651.) 

CuBr2,  3NH3.  Completely  sol.  in  a  little 
H2O,  but  is  decomp.  by  dilution.  Insol.  in 
alcohol.  (Rammelsberg,  Pogg.  55. 246.) 

CuBr2,  4NH3+H2O.  100  pts.  H2O  dis- 
solve 69.03  pts.  CuBr2,  4NH3  at  25°.  (Pud- 
schies,  Dissert.) 

CuBr2,  5NH3.  As  above.  (Rammels- 
berg.) 

CuBr2,  6NH3.  Sol.  in  small  amts.  of  H20, 
but  decomp.  on  dilution.  (Richards.) 

Cupric  bromide  nitric  oxide,  CuBr2,  NO. 

Decomp.  by  H2O.  (Manchot,  B.  1914, 
47.  1607.) 

Cuprous  chloride,  Cu2Cl2. 

1.53  g.  Cu2Cl2  dissolve  in  100  g.  H2O  at 
21.5°;  1.55  g.  at  26.5°.  (Kremann  and  Noss, 
M.  1912,  33.  1206.) 

Solubility  of  Cu2Cl2  in  H2O  in  an  atmosphere 

of  hydrogen. 
Solubility  is  recorded  in  mg-atoms  per  1. 


t° 

20^2 
19.6 
19.3 

Total 
Cu 

CuCl2 
by 
analysis 

Cl 

CU2C12 

calc. 

Cu2Cl2 

by 

analysis 

2.752 
2.919 
2.971 
2.861 

2.124 
2.254 
2.294 
2.245 

5.672 
5.525 
5.464 
5.464 

0.628 
0.665 
0.677 
0.616 

0.420 
0.474 
0.499 

(Bodlander,  Z.  anorg.  1902,  31.  12.) 

Solubility  of  Cu2Cl2  in  H2O  in  an  atmosphere 

of  CO,. 
Solubility  is  recorded  in  mg-atoms  per  1. 


t° 

Tolal 
Cu 

CuCl2 
by 

analysis 

Cl 

Cu2Cl2 

by. 

analysis 

Cu2Cl2 
calc. 

20.6 
21.7 

19> 

2.818 

2.805 
2.880 
2.805 

2  '243 

2.258 
2.138 

5.235 
5.430 
5.312 
5.390 

0.525 
0.516 
0.391 
0.336 

0^562 
0  662 
0.667 

(Bodlander,  1.  c.) 

Sol.  in  cone.  HCl+Aq;  insol.  in  dil.  HNO3, 
or  H2SO4+Aq.  Not  attacked  by  cold  cone. 
H2SO4,  and  only  si.  on  warming.  (Rosen- 
feld,  B.  12.  954.)  Sol.  in  NH4OH+Aq;  sol. 
in  hot  NaCl,  KC1,  FeCl3,  ZnCl2,  MnCl2,  etc. 
+Aq.  1  mol.  Na2S2O3  in  aqueous  solution  dis- 
solves 1  mol.  Cu2Cl2.  (Winklrr,  J.  pr.  88. 
428.)  Sol.  inKI,  I2,  KCN,  or(NH4)2SO4  + 
Aq.  (Renault,  C.  R.  59.  558.) 


Solubility  in  HCl+Aq  at   17°. 


Cu2Cl2 


Y<z  mols.  CuCl2  in  mgs.  in  10  ccm.  solu- 
tion.   HCl  =  mols.  HCl  in  ditto. 


Cu2Cl2 
2 

HCl 

Sp.  gr. 

0.475 
1.4 
1.575 
4.5 

8.25 
11.5 

8.975 
15.7 
18.2 
34.5 
47.8 
57.0 

1.050 

iloso 

1.135 

(Chatelier,  calc.  by  Engel,  A.  ch.  (6)  17.  377.) 
Solubility  of  Cu2Cl2  in  HCl+Ar  at  0°. 


Cu2Cl2 
2 

HCI 

Sp.  gr. 

1.5 
2.9 
8.25 
15.5 
33.0 

17.5 
26.0 
44.75 
68.5 
104.0 

1.049 
1.065 
1.132 
1.261 
1.345 

(Engel,  I.  c.) 

Freshly  pptd.  Cu2Cl2  is  sol.  in  H2SO3+Aq. 
(Lean  and  Whatmough,  Chem.  Soc.  1898, 
73.  150.) 

SI.  sol.  in  normal  NH4OH+Aq  only  by 
shaking  several  hours,  a  0.02  normal  solution 
of  cuprous  copper  being  obtained.  (Gaus, 
Z.  anorg.  1900,  25.  258.) 

Insol.  in  Na2S2O6+Aq.  (Siewert,  Gm.  K. 
5.  1,  893.) 

Sol.  in  alkyl  triphosphites.  (Arbusoff, 
C.  C.  1906,  II.  750.) 

Solubility  in  FeCl2,  4H2O+Aq  at  21.5°. 


In  100  g.  H2O 

Solid  phase 

g.  FeCl2 

g.  Cu2Cl2 

1.535 

CujCU 

e.ois 

1.33 

11.62 

1.81 

16.30 

3.11 

26.305 

7.125 

29.35 

8.06 

33.125 

9.565 

43.75 

12.44 

54  00 

17.04 

66.40 

21.60 

• 

73.20 

23.20 

Cu2Cl2+FeCl2,  4H20 

71.895 

21.655 

FeCl2,  4H2O 

69.34 

11.895 

n 

65.10 



u 

(Kremann  and  Noss,  M.  1912,  33.  1208.) 

296 


CUPROUS  CHLORIDE 


Solubility  of  Cu2Cl2  in  KCl+Aq  at  t°.    De- 

Solubility of  Cu2Cl2+KCl  in  H2O  at  22°.— 

termined  in  an  atmosphere  of  CO2. 

Continued 

t° 

g.  mol.  KCl  per  1. 

g.  atoms  Cu  per  1. 

G.  in  1  g.  of  solution 

18.3 

0.05 

0.002411 

CU2C12 

KCl 

Solid  Phase 

16 

0  1 

0  004702 

16 

\J  .  X 

0.2 

Oi  009458 

0.1621 

0.2330 

Cu2Cl2 

19.2 

1.0 

0.0970 

0.1723 

0.2384 

tt 

16.4 

2.0 

0.3840 

0.1907 

0.2374 

u 

001  AS 

OOPJ1  A 

(f 

(Bodlander  and  Storbeck,  Z.  anorg.  1902,  31. 

.  ZL<to 

0.2145 

.^OlD 

0.2506 

Cu2Cl2-f  Cu2Cl2,  4KC1 

17.) 

0.2149 

0.2549 

Cu2Cl2,  4KC1 

0  .  1548 

0  .  2387 

ft 

Solubility  of  Cu2Cl2  in  KCl+Aq  at  t°.    De- 
termined in  an  atmosphere  of  CO2. 

o!l473 
0  1399 

0  12363 
0  2357 

tt 

(t 

All  values  recorded  in  millimols  per  litre. 

o!l439 

0.2389 

ii 

0.1451 

0.2363 

tt 

t° 

KCl 

Cupric 

Total 

Cuprous 
copper 

Cl 

0.1155 

0.2320 

tt 

copper 

copper 

calc. 

0.1139 

OAOKQ 

0.2350 

OOO  K.C\ 

it 

K 

20° 

0 

2.222 

2.851 

0.629 

5.436 

.uyoo 
0.0735 

.  Jooy 
0.2349 

(t 

19 

1 

1.901 

2.385 

0.484 

5.287 

0.0555 

0.2389 

tt 

19 

2 

1.571 

2.150 

0.589 

5.614 

O.C453 

0.2404 

K 

19 

2.5 

1.421 

1.955 

0.534 

6.015 

0.0366 

0.2433 

H 

19 

3 

1.523 

1.983 

0.460 

6.247 

0.0314 

0.2503 

(( 

16 

5 

1.008 

1.522 

0.514 

7.525 

0.0285 

0.2499 

(t 

18 

10 

0.475 

1.236 

0.761 

11.735 

0.0265 

0.2523 

f( 

20 

15 

0.322 

1.344 

1.022 

16.437 

0.0220 

0.2628 

(I 

19 

20 

0.324 

1.446 

1.122 

21.356 

0.0193 

0.2687 

( 

19 

30 

0.1308 

1.761 

1.630 

31.911 

0.0176 

0.2698 

( 

18 

50 

0.1088 

2.411 

2.302 

0.0193 

0.2703 

Cu2Cl2,  4KC1+KC1 

16 

100 

0 

4.702 

4.702 

0.0160 

0.2706 

KCl 

16 

200 

0 

9.485 

9.485 

.  .  . 

0.0124 

0.2668 

t 

19 

1000 

0 

97.0 

97.0 

0.0058 

0.2632 

< 

16 

2000 

0 

384.0 

384,0 

... 

0.0000 

0.2568 

t 

(Bodlander  and  Storbeck,  Z.  anorg.  1902,  31. 
24.) 

Solutions  of  0.05=0.4  normal  KCl  dis- 
solve Cu2Cl2  with  the  formation  of  KCuCl2; 
those  of  higher  concentration  with  the  forma- 
tion of  K2CuCl3.  (Bodlander  and  Storbeck, 
Z.  anorg.  1902,  31.  41.) 

Solubility  of  Cu2Cl2+KCl  in  H20  at  22°. 


G.  in  1  g.  of  solution 

Solid  Phase 

Cu2Cl2 

KCl 

0.00115 

0.0387 

Cu2Cl2 

0.00405 

0.0656 

0.00861 

0.0824 

0.0137 

0.0984 

0.0219 

0.1133 

0.0390 

0.1406 

0.0484 

0.1530 

0.0675 

0.1639 

0.0719 

0.1747 

0.0863 

0.1839 

0.1043 

0.2027 

0.1084 

0.2018 

0.1021 

0.2031 

0.1204 

0.2095 

u 

0.1332 

0.2164 

u 

(Bronsted,  Z.  phys.  Ch.  1912,  80.  208.) 


Solubility  in  NaCl+Aq. 

Sat.  NaCl+Aq  dissolves  16.9  %  Cu2Cl2  at 
90°;  11.9  %  at  40°;  and  8.9  %  at  11°. 

15  %  NaCl+Aq  dissolves  10.3  %  Cu2Cl2  at 
90°;  6.0  %  at  40°;  and  3.6  %  at  14°. 

5%  NaCl-j-Aq  dissolves  2.6  %  Cu2Cl2  at 
90°,  and  1.1  %  at  40.°  (Hunt,  Sill.  Am.  J. 
(2)  49.  154.) 


Solubility  in  NaCl+Aq  at  26.5°. 


In  100  g.  H2O 

Solid  phase 

Cu2Cl2 

NaCl 

1.55 

Cu2Cl2 

3.15 

10.80 

a 

7.30 

20.70 

tt 

40.60 

27.00 

1C 

49.10 

36.48 

tt 

57.21 

44.14 

Cu2Cl2+NaCl 

41.40 

55.95 

NaCl 

18.70 

50.90 

ft 

(Kremann  and  Noss,  M.  1912,  33.  1210.) 


CUPRIC  CHLORIDE 


297 


Solubility  of  Cu2Cl2  in  CuS04-fAq  at  t°. 
Values  recorded  in  millimols  per  1. 

Sat.  CuCl2+Aq.  contains  at: 
-20°     -5°       4-12°     17°      32° 
37         38.8    39.3      41.7    43.2%CuCl2, 
39°        55°       68°        73°       91° 
44.0     46.5    47.9      48.6    51.0%CuCl2. 
(fitard,  A.  ch.  1894,  (7)  2.  536.) 

Sp.  gr.  of  CuCl2+Aq  at  17.5°. 

t° 

19.7 
16.3 
18.6 
17.5 
19.4 
20.4 
20.5 
20.1 

Cone,  of 
CuSOi 

Cupric 
copper 

Total 
copper 

Cuprous 
copper 
calc. 

Cl 

5.312 
4.805 
4.908 
4.530 
4.687 
4.287 
4.256 
4.329 

0.49375 
0.9875 
1.4812 
1  975 
2.4687 
2.9625 
4.9375 

2.258 
2.746 
3.145 
3.315 
4.131 
4.349 
4.625 
6.546 

2.880 
3.125 
3.602 
3.915 
4.553 
4.786 
5.193 
7.276 

0  622 
0.379 
0.457 
0.600 
0.422 
0.437 
0.509 
0.730 

%  CuCh 

Sp.  gr. 

%  CuCh 

Sp.  gr. 

5 
10 

15 
20 

1.0455 
1.0920 
1.1565 
1.2223 

25 
30 
35 

40 

1.2918 
1.3618 
1.4447 
1.5284 

(Bodlander  and  Storbeck,  Z.  anorg.  1902,  31. 

22.) 

(Franz,  J.  pr.  (2)  5.  274.) 

Insol.  in  SbCl3.  (Klemensiewicz,  Bull. 
Acad.  Crac.  1908,  6,  485.) 

SI.  sol.  in  liquid  NH3.  (Franklin,  Am. 
Ch.  J.  1898,  20,  827.) 

Insol.  in  alcohol. 

SI.  sol.  in  ether.    (Gehlen.) 

Sol.  in  quinoline.  (Beckmann  and  Gab  el, 
Z.  anorg.  1906,  61.  236.) 

Sol.  in  pyridine.  (Schroeder,  Dissert. 
1901.) 

Insol.  in  phosgene.  (Eidmann,  Dissert. 
1899.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329.) 

Insol.  in  acetone  and  in  methylal.  (Eid- 
mann, C.  C.  1899,  II.  1014.) 

Difficultly  sol.  in  methyl  acetate.  (Nau- 
mann, B.  1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Alexander,  Dis- 
sert. 1899.)  (Naumann,  B.  1904,  37.  3601.) 

Difficultly  sol.  in  ethyl  acetate.  (Nau- 
mann, B.  1910,  43.  314.) 

100  g.  acetonitrile  dissolve  13.33  g.  Cu2Cl2 
at  18°.  (Naumann  and  Schier,  B.  1914,  47. 
249.) 

Sol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1369.) 

Sol.  in  hot  benzonitrile  and  other  aro- 
matic nitriles.  (Werner,  Z.  anorg.  1897,  16. 

Mol.  weight  determined  in  pyridine 
methyl  and  ethyl  sulphides.  (Werner,  Z. 
anorg.  1897,  15.  19,  25  and  28.) 

Min.  Nantokite.  Sol.  in  HC1,  HNO8,  or 
NH4OH+Aq. 

Cupric  chloride,   CuCl2. 

Deliquescent.  100  pts.  H2O  dissolve  70.6 
pts.  CuCl2  at  0°;  100  pts.  CuCl2+Aq  contain 
41.4  pts.  CuCl2.  (Engel,  A.  ch.  (6)  17.  350.) 

100  pts.  H2O  dissolve  76.2  pts.  CuCl2  at 
16.1°,  or  100  pts.  CuCl2+Aq  sat.  at  16.1°  con- 
tain 43.25  pts.  CuCl2.  (Rudorff,  B.  6.  484.) 

100  pts.  CuCl2+Aq  sat.  at  17°  contain 
43.06  pts.  CuCl2;  at  31.5°,  contain  44.7  pts. 
CuCl2.  Coefficient  of  solubility  =  4 1.4  + 
O.lOSt.  (Reicher  and  Deventer,  Z.  phys. 
Ch.  5.  560.) 


Sp.  gr. 


of  CuCl2+Aq  at  22.9°,  containing  in 
1000  g.  H2O,  g.  CuCl2+2H2O. 


85.5  (  =  %  mol.)  171       255.5  g.  CuCl2+2H2O, 

1.057 

1.108     1.154 

342 

427.5     '    513          g.  CuCl2+2H2O, 

1.197 

1.238         1.275 

598.5 

684          g.  CuCl2+2H2O, 

1.309 

1.341 

769.5 

855          g.  CuCl2+2H20, 

1.371 

1.399 

940.5 

1.026       g.  CuCl2+2H20. 

1.425 

1.449 

Containing  CuCl2  (anhydrous). 


1.059 

337.5 
1.257 

540 
1.379 


135     202.5 
1.114   1.165 

270g.CuCl2, 
1.213 

405      472.5r 
1.299    1.30 

g.  CuCl2. 

607.5   675 
1.416    1.453 

g.  CuCl2. 

(Gerlach,  Z.  anal.  28.  468.) 


Sp.  gr.  of  CuCl2+Aq  at  0°.  S=pts.  CuCl2 
in  100  pts.  solution;  Si  =  mols.  CuCl2  in 
100  mols.  of  solution. 


s 

Si 

Sp.  gr. 

39.4170 
35.3839 
30.9255 
26.1129 
20.6697 
14.5820 
8.0732 

8.00 
6.82 
5.65 
4.51 
3.36 
2.23 
1.16 

1.4797 
1.4173 
1.3529 
1.2881 
1.2204 
1  .  1494 
1.0796 

(Charpy,  A.  ch.  (6)  29.  25.) 

Tables  for  7°,  30.5°,  49.2°,  and  65°  are  also 
given  by  Charpy. 

Sp.  gr.  of  CuCl2+Aci  at  room  temp., 

containing: 

12.006      21.349      33.027%  CuCl2. 
1.1037      1.2154      1.3312 
(Wagner,  W.  Ann.  1883,  18.  273.) 


298 


CUPRIC  CHLORIDE 


Sp.  gr.  at  20°  of  CuCl2+Aq  containing  M. 

mols.  CuCl2  per  liter. 

M.  0.01  0.05  0.075 

Sp.gr.       1.001208       1.00637         1.009264 
M.  0.10  0.20  0.50 

Sp.gr.       1.012614       1.030991         1.051479 
M.  0.75  1.0 

Sp.gr.      1.090912  1.120249 

M.  1.5  2.0 

Sp.gr.       1.177618  1.234551 

(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38.  717.) 
Sp.  gr.  of  CuCl2+Aq  at  25°. 


Concentration  of  CuCl2  +Aq. 

Sp.  gr. 

1  —  normal 

Vr-     " 

V4—          " 

Vs—       " 

1.0624 
1.0313 
1.0158 
1.0077 

(Wagner,  Z.  phys.  Ch.  1890,  5.  38.) 

Much  less  sol.  in  HCl+Aq  than  in  H2O. 
1  1.  HCl+Aq  containing  45  pts.  HC1  to  100 
pts.  H2O  dissolves  only  290  g.  CuCl2  at  12°, 
whereas  1 1.  H2O  at  12°  dissolves  630  g.  CuCl2. 
(Ditte,  C.  R.  1881,  92.  353.) 

Solubility    in    HCl+Aq    at    0°.     CuCl.  ^ 

%  mols.  in  milligrammes  in  10  ccm. 
solution.  HCl  =  mols.  HC1  in  ditto:  H2O 
=  g.  H,0. 


CuCl2 

Sum  of 

2 

HCl 

equiv  . 

Sp.  gr. 

H2O 

91.75 

0 

91.75 

1.490 

8.73 

86.8 

4.5 

91.3 

1.475 

8.74 

83.2 

7.8 

91 

1.458 

79.35 

10.5 

89.85 

1.435 

8^64 

68.4 

20.25 

88.65 

.389 

8.56 

50.0 

37.5 

87.5 

.319 

8.47 

22.8 

70.25 

93.05 

.231 

8.21 

23.5 

102.5 

126 

.288 

7.56 

26.7 

128 

154.7 

.323 

6.77 

(Engel,  A.  ch.  (6)  17  351.) 

Not  decomp.  by  cold  H2  SO4. 
Sol.   in  NH4Cl+Aq.     Very  sol.   in   cone. 
NaCl+Aq.    (Boussingault.) 

Solubility  of  CuCl2  in  NH4Cl+Aq  at  30°. 


% 

NH4C1 

Cu6i2 

Solid  phase 

29.5 

0 

NH4C1 

28.6 
12.1 
2.03 

1.9 

15.6 
43.2 

NH4Cl+CuCl2,  2NH4C1,  H2O 
CuCl2,  2NH4C1,  HoO 
CuCl2,  2NH4C1,  H20+CuCl2, 

2H20 

0 

43.95 

CuCl2,  2H2O 

(Schreinemakers,  Z.  phys.  Ch.  1909,  66.  688.) 
See  also  NH4Cl+CuCl2  under  ammonium 
chloride. 


Solubility  of  CuCl2+HgCl2  in  H2O  at  35°. 


%  HgCl2 


0 

21.03 
37.30 
44.47 
50.47 
52.44 
52.54 
52.81 
51 . 03 
49.50 
23.87 

8.51 


%  CuCU 


44.47 

33.50 

26.07 

23.31 

21.50 

19.40 

18.46 

18.06 

14.73 

5.94 

2.64 

8.51 


Solid  Phase 


CuCl2,  2H20 


CuCl2+HgCl2 
HgCl2 


(Schreinemakers  and  Thonus,  Proc.  K.  Akad. 
Wet.  1912,  16.  472.) 

Solubility  of  CuCl2+KCl  in  H2O  at  t°. 


Cl  per  g. 
of  solution 

Mols.  per 
100  mols. 
H20 

t° 

0 

i 

1 

o 

u 

to 

6 

M 

39.4 

0.120 

0.107 

5.56 

9.93 

CuCl2,  2KC1.2H2O  + 

KC1 

49.9 

0.129 

0.115 

6.39 

11.4 

"              111'"! 

60.4 

0.142 

0.125 

7.71 

13.6 

" 

79.1 

0.168 

0.142 

11.1 

18.8 

" 

90.5 
93.7 

0.188 
0.194 

0.154 
0.156 

14.9 
16.2 

24.4 
26.0 

CuCh,  KC1+KC1 

98.8 
0 

0.197 
0.214 

0.162 
0.021 

17.5 
9.84 

28.7 
1.94 

CuCl2,  2KC1.2H2O  + 

CuCl2.3H20 

39.6 

0.232 

0.049 

12.9 

5.44 

" 

50.1 

0.233 

0.059 

13.7 

6.90 

** 

52.9 
60.2 

0.241 
0.246 

0.062 
0.066 

14.8 
15.8 

7.63 
8.49 

CuCl2,  KC1  +CuCl2. 

2H20 

72.6 

0.255 

0.063 

16.8 

8.35 

*' 

64.2 

14.9 

11.6 

CuCl2,  2KC1.2H20  + 

CuCl2,  KC1 

72.5 

14.8 

1.50 

CuCl2,  KC1 

(Meyerhoffer,  Z.  phys.  Ch.  1890,  5.  102.) 

100  g.  H2O  dissolve  72.6  g.  CuCl2+16.  Og 
NaCl.    (Rudorff,  B.  6.  684.) 

Solubility  of  CuCl2+NaCl  in  H2O  at  30°. 


%  NaCl 

%  CuCl2 

Solid  Phase 

0 

43.95 

CuCl2,2H2O 

3.10 

41.14 

4.28 

41.06 

6.41 

39.40 

10.25 

36.86 

CuCl2 

fNaCl 

12.02 

32.38 

Ni 

Cl 

12.25 

32.40 

13.54 

28.64 

15.40 

23.72 

18.44 

16.98 

20.61 

11.03 

26.47 

0 

(Schreinemakers  and  de  Baat,  Z.  phys.  Ch. 
1909,  65.  586.) 


CUPRIC  CHLORIDE 


299 


Solubility  of  CuCl2  in  CuSO4+Aq  at  30°. 

Easily  sol.  in  acetone.    (Krug  and  M'Elroy, 
J.  Anal.  Ch.  6.  184.) 
Insol.  in  benzene. 

Solubility  in  organic  solvents. 

Composition  of  the 
solution 

Solid  phase. 

% 
bv  wt. 
CuCh 

%by 
CuS 

wt 

34 

Solvent 

t° 

Sat.  solution 
contains  % 
CuCh 

0 
6.58 
15.68 
25.67 
39.48 
42.77 
42.47 
43.25 
43.95 

20.32 
13.62 
8.93 
4.77 
3.21 
2.89 
2.90 
1.14 
0 

CuSO4,  5H2O 

u 
11 
If 
(( 

CuS04,  5H2O+CuClo,  2H2O 

K 

CuCl2,  2H2O 

u 

Methyl  alcohol 

22 
40 
50 
60 

36.8 
37.5 
37.1 
37.5 

Abs.  ethyl  alcohol 

0 
19 
20 
38 
50 

32.0 
35.7 
35.9 
38.5 
41.7 

(Schreinemakers,  Z.  phys.  Ch.  1909,  69.  561.) 

Insol.  in  liquid  NH3.     (Gore,  Am.  Ch.  J. 
1898,  20.  827.) 
SI.  sol.  in  liquid  HF.    (Franklin,  Z.  anorg. 
1905,  46.  2.) 
Sol.  in  alcohol  and  ether. 
Sol.  in  1  pt.  strong  alcohol. 
100  pts.  absolute  methyl  alcohol  dissolve  68 
pts.  CuCl2  at  15.5°;  100  pts.  absolute  ethyl 
alcohol  dissolve  53  pts.  CuCl2  at  15.5°.     (de 
Bruyn,  Z.  phys.  Ch.  10.  783.) 
See  also  under  CuCl2+2H2O. 

Solubility  of  CuCl2+KCl  in  absolute  alcohol 
at  25°. 

Propyl  alcohol 

—  15 
19 
37 
57 
62 

26.8 
30.9 
30.7 
30.3 
30.5 

Allyl  alcohol 

-20 

-   4 
27 
32 

23.4 
23.6 
22.9 
23.3 

N-butyl  alcohol 

0 
23 
37 
55 

84. 
92 

15.2 
15.8 
15.7 
16.1 
16.2 
16.7 

°7 
CuClt 

KCl 

Solid  Phase 

1.27 
1.51 
2.15 
5.25 
30.16 
34.17 
34.45 
34  29 
33.97 

0.28 
0.28 

0.2! 

0.21 
0.21 
0.00 

! 

KC1+KC1,  CuCl2 

a 

KCl,CuCl2 
a 
KCl,  CuClo+CuClo,  C2H6OH 

a 
it 

CuCl2,  C2H5OH 

Ethyl  formate 

-20 

+24 
37 
50 

10.2 
9.4 
7.4 

7.2 

Ethyl  acetate 

+20 
40 

72 

3.0 
2.5 
1.3 

(Foote  and  Walden,  J.  Am.  Chem.  Soc.  1911. 
33.  1032.) 

Solubility  of  CuCl2+KCl  in  acetone  at  25°. 

Acetone 

—  20 

+  8 

18.4 
18.8 

% 
CuCl2 

$, 

Solid  Phase 

Isopropyl  alcohol 

32 
70 

84 

11.0 

28.3 
28.7 

0.34 
0.48 
1.50 
2.06 
2.49 
2.32 

0.38 
6!27 

KC1+KC1,  CuCl2 

KCl,  CuCl2 

a 

(i 
KCl,  CuCl2+CuCl2,  C3H6O 

(fitard,  A.  ch.  1894,  (7)  2.  565.) 
See  also  under  CuCl2+2H2O. 

1  g.  CuCl2  is  sol.  in  181  g.  methyl  acetate 
at  18°.    Sp.  gr.  18°/4°  of  the  sat.  solution  = 
0.939.     (Naumann,  B.  1909,  42.  3793.) 
1  g.  CuCl2  is  sol.  in  249  g.  ethyl  acetate 
at  18°.    Sp.  gr.  of  sat.  solution  18°/4b  =  0.9055. 
(Naumann,  B.  1904,  37.  3603.) 
Difficultly  sol.   in   ethyl   acetate.     CNau- 
mann,  B.  1910,  43.  314.) 

(Foote  and  Walden,  J.  Am.  Chem.  Soc.  1911, 
33.  1032.) 

100  g.  of  sat.  solution  of  CuCl2  in  ethyl 
alcohol  contains  33.97  g.  CrCl2.    (Foote  and 
Walden,  J.  Am.  Chem.  Soc.  1911,  33.  1032.) 

300 


CUPRIC  CHLORIDE 


1  pt.  sol.  in  249.3  pts.  ethyl  acetate  at  10°. 
(Alexander,  Dissert.  1899.)  " 

Solubility  in  acetone. 

34.7  g.  acetone  dissolve  1  g.  CuCl2  at  18°. 
Sp.  gr.  of  sat.  solution  18°/4°  =0.8154.  (Nau- 
mann,  B.  1904,  37.  4329.) 

1.40  pts.  are  sol.  in  100  pts.  acetone  at  56°. 
(Laszczynski,  B.  1894,  27.  2287.) 

Sol.  in  acetone  and  methylal.  1  gram,  dis- 
solves in  34.08  grams  of  acetone  at  18°. 
(Eidmann,  C.  C.  1899,  II,  1014.) 

100  pts.  absolute  ether  dissolve  0.043  g. 
CuCl2.  (Bodtker,  Z.  phys.  Ch.  1897,  22. 
511.) 

Mol.  weight  determined  in  pyridine  and 
methyl  sulphide.  (Werner,  Z.  anorg.  1897, 
16.  20  and  25.) 

100  g.  sat.  solution  in  acetonitrile  contains 
1.57  g.  CuCl2.  (Naumann  and  Schier,  B. 
1914,  47.  249.) 

SI.  sol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1369.) 

Sol.  in  boiling  dipropylamine.  (Werner, 
Z.  anorg.  1897, 16.  34.) 

Sol.  in  urethane.  (Ley,  Z.  phys.  Ch.  1897, 
22.  81);  (Castoro  Z.  anorg.  1899,  20,  61.) 

+H2O.    (Ditte,  A.  ch.  (5)  22.  551.) 

Sol.  in  H2O  with  slight  decomp.  (Sabatier, 
Bull.  Soc.  1895,  (3)  13.  601.) 

+2H2O.  Deliquescent.  100  g.  H2O  dis- 
solve 121.4  g.  CuCl2+2H2O  at  16.1°.  (Rtt- 
dorff.) 

Aq.  sol.  at  35°  contains  9.689  Mol.  %  CuCl2. 
"  15°        "        8.934     "      %       " 

(Schreinemakers,  C.  C.  1911,  II.  349.) 

P"CuCl2+2H20+Aq.  sat.  at  30°  contains 
43.95%  CuCl2.  (Meerburg,  C.  C.  1904,  II. 
1362.) 

43.95  g.  anhydrous  CuCl2  are  dissolved  in 
100  g.  CuCl2+Aq  at  30°.  (Schreinemakers, 
Arch.  neer.  Sc.  1910  [2],  15.  117.) 

44.47%  by  weight  anhydrous  CuCl2  is  dis- 
solved in  H2O  at  35°.  (Schreinemakers  and 
Thonus;  Verh.  k.  Akad.  Wet.  Amst.  1912, 
21.  333.) 


Solubility  of  CuCl2+2H2O  in  ethyl  alcohol 
+Aq  at  11.5°. 


Percent  of  ethyl  alcohol 
by  volume 

Grams  CuCla  dissolved 
in  5  cc. 

99.3 
98.3 
96.3 
95.3 
94.3 

1.175 
1.116 
1.097 
1.070 
1.059 

Anhydrous  salt  dissolves  readily  in  absolute 
ethyl  alcohol;  CuCl2+2H2O  is  precipitated 
by  H2O. 


Solubility  of  CuCl2+2H2O  in  ethyl  alcohol  + 
Aq  at  11.5°  C.  under  addition  of  in- 
creasing amounts  of  CuCl2. 
P  =  Percent  of  ethyl  alcohol  by  volume. 
G  =  Grams  of  CuCl2  added. 
Cc  =  Grams  of  CuCl2  in  5  cc..of  the  solution. 
Cw  =  Grams  of  water  in  5  cc.  of  the  solution, 
calculated  from 

(1)  the  water  content  of  the  alcohol. 

(2)  the  water  of  crystallization  which  had 

gone  into  solution. 

(3)  the  water  held  mechanically  in  CuCl2 

+2H2O. 


p 

G 

Cw 

Cc 

89.3 

0.000 

0.794 

1.137 

90.3 

0.744 

1.122 

91.3 

0.695 

1.104 

92.3 

0.648 

1.090 

94.3 

0.561 

1.096 

95.3 

0.517 

1.095 

96.3 

0.478 

1.116 

97.3 

0.440 

1.140 

98.3 

0.396 

1.194 

99.3 

0.369 

1.208 

0.223 

0.330 

1.295 

0.444 

0.290 

1.395 

0.665 

0.270 

1.506 

0.887 

0.247 

1.639 

1.106 

0.223 

1.772 

1.324 

0.205 

1.921 

1.540 

0.191 

2.086 

1.739 

0.179 

2.236 

1.957 

0.164 

2.400 

(Bodtker,  Z.  phys.  Ch.  1897,  22.  506-507.) 

100  pts.  absolute  ether  dissolve  0.061  g. 
CuCl2+2H2O.  (Bodtker,  Z.  phys.  Ch.  1897, 
22.  511.) 

0.11  pts.  are  sol.  in  100  pts.  ether  at  16°. 
0.11  "  "  "  "  100  "  "  "  35°. 
8.86  "  "  "  "  100  "  acetone "  0°. 
8.92  "  "  "  "  100  "  "  "  13.5°. 
(Laszczynski,  B.  1894,  27.  2286  and  2287.) 

Solubility  in  organic  solvents  at  t°. 


Pts.  of 

solvent 

required 

to  dis- 

Solvent 

t° 

solve 

1  pt. 
CuCl2-f- 

2H20 

at  t°. 

Pure  methyl  alcohol 

20° 

7.3 

" 

18.9 

7.6 

Ethyl  alcohol  (95°) 

20.3 

11.6 

" 

19.6 

11.9 

Pure  acetone 

22.1 

43.6 

" 

20.0 

44.2 

90  pts.  ethyl  alcohol  (98°)  +10  pts. 

H2O 

21.8 

9.0 

" 

23.0 

8.5 

CUPROUS  SODIUM  CHLORIDE 


301 


Solubility  in  organic  solvents  at  t°.  —  Cont. 

CuCl2,  2HC1.    Deliquescent.    Verv  sol.  in 

H2O.    (Alexander,  Dissert.  1899.) 

Pts.  of 

solvent 

+5H2O.      Properties     as    above.       (Sa- 

Solvent 

t° 

required 
to  dis- 
solve 
1  pt. 

batier.  C.  R,  106.  1724.) 
CuCl2,3HCl.     Sol.  in  H2O.     (Neumann 
M.  1894,  16.  493.) 

CuCl2  + 
2H20 

Cupric    gold     (auric)     chloride,     CuCl2, 

att° 

2AuCl3+6H2O. 

80  pts.  abs.  alcohol  +20  pts.  H>O 

28.1 
20.7 

6.0 
6.2 

10%  is  sol.  in  H2O  at  18°.     (Mylius,  Z. 
anorg.  1911,  70.  210.) 

80  pts.  acetone  +20  pts.  H2O 

23.1 
21.8 

5.3 
5.6 

Cupric    lithium     chloride,     CuCl2,     LiCl  + 

80  pts.  acetone  +20  pts.  methyl 
alcohol 

10  pts.  methyl  alcohol  +90  pts. 

23.1 
24.0 

12.0 
11.6 

Decomp.  on  air.    Decomp.  by  dissolving  in 
H20  .   Sol  .  in  cone  .  LiCl  +  Aq  without  decomp  . 
Decomp.  by  alcohol.     (Chassevant,  A.  ch. 
(6)  30.  33.) 

ethyl  alcohol  (98°) 

24.2 
25.0 

5.4 
5.1 

+2H20'.    (Meyerhoffer,  W.  A.  B.  100,  2b. 

621.) 

20  pts.  methyl  alcohol  +80  pts.  ord. 

ether 

24.1 

15.1 

Cupric  mercuric  chloride. 

80  pts.  abs.  alcohol  +20  pts.  ord. 

22.4 
24.1 

15.7 

8.8 

Easily  sol.  in  H20.    (v.  Bonsdorff.) 

ether 

Cupric  mercuric  potassium  chloride,  CuCl2, 

" 

25.0 

8.5 

3HgCl2,  6KC1+2H2O. 

Comm.  methyl  alcohol 
85  pts.  pyridine+15  pts.  H2O 

23.9 
23.0 
24.4 

5.4 
5.6 
63.4 

Deliquescent  in  moist  air.    Sol.  'in  boiling 
H2O  without  decomp.,  and  recrystallises  if 
cooled  slowly.     Insol.   in  absolute  alcohol. 

60  pts.  pyridine+40  pts.  H2O 

23.6 
27.3 

63.7 
26.7 

(v.  Bonsdorff,  Pogg.  33.  81.) 

75  pts.  a  picoline  +25  pts.  H2O 
70  pts.  a  picoline  +30  pts.  H2O 

28.0 
26.1 
25.1 
26.1 

26.2 
51.6 
52.3 
47.3 

Cuprous  nitrosyl  chloride,  Cu2Cl2,  2NOC1. 
Very  deliquescent  and  sol.  in  H2O  with  im- 
mediate decomp.     (Sudborough,  Chem.  Soc. 
59.  658.) 

(de  Coninck,  C.  R.  1900,  131.  59.) 

Solubility  in  organic  solvents. 

Sol.  in  propyl  alcohol,  hot  glycol,  hot 
glycerine,  hot  paraldehyde,  hot  crys.  acetic 
acid,  pure  acetone,  30%  methylamine+Aq, 
pure  pyridine,  pure  a-picoline,  acetonitrile; 
si.  sol.  in  isobutyl  and  amyl  alcohols,  crystal- 
lizable  formic  acid,  ethyl  acetate;  insol.  in 
cold  glycol,  cold  glycerine,  cold  paraldehyde, 
benzaldehyde,  cold  crystallizable  acetic  acid, 
ord.  ether,  abs.  ether,  hot  and  cold  CS2,  cold 
aniline,  cold  orthotoluidine,  methylene  chlor- 
ide, ethyl  iodide,  propyl  iodide,  ethylene 
bromide,  benzene,  toluene,  xylene,  ligroin, 
nitrobenzene,  cold  piperidine  and  essence  of 
terebenthine.  (de  Coninck,  C.  R.  1900,  131. 
•59.) 

+5H20. 

Aq.  sol.  at  35°  contains  2.921  Mol.  %  CuCl2. 

15°       "        1.11 
(Schreinemakers,  C.  C.  1911,  II.  349.) 

Cuprous  hydrogen  chloride,  CuCl,HCl. 
Sol.  in  H2O.    (Neumann,  M.  1894, 15.  493.) 

Cupric  hydrogen  chloride,  CuCl2,  HC1+3H2O 
Decomp.  by  H2O.    Sol.  in  HCl+Aq  below 
0°    .(Engel,  C.  R.  106.  273.) 


Cuprous  potassium  chloride,  Cu2Cl2,  4KC1. 
Sol.  in  H2O.  (Mitscherlich,  A.  ch.  73.  384.) 
For  solubility  data,  see  Cu2Cl2+KCl  under 

cuprous  chloride. 

Cupric  potassium  chloride. 

CuCl2,KCl.  (Meyerhoffer,  Z.  phys.  Ch.  3. 
336.) 

Sol.  in  H2O;  only  si.  sol.  in  cone.  HCl+Aq. 
(Groger,  Z.  anorg.  1899,  19.  330.) 

CuCl2,  2KC1+2H2O.  Sol.  in  H2O  and 
alcohol.  (Berzelius,  Pogg.  13.  458.) 

The  composition  of  the  hydrates  formed  by 
this  salt  at  different  dilutions  is  calculated 
from  determinations  of  the  lowering  of  the 
fr.  pt.  produced  by  the  salt  and  of  the  con- 
ductivity and  sp.  gr.  of  its  aqueous  solutions. 
(Jones,  Am.  Ch.  J.  1905,  34.  322.) 

For  solubility  data,  see  CuCl2+KCl  under 
cupric  chloride. 

Cupric  rubidium  chloride,  CuCl2,  2RbCl. 

Easily  sol.  in  H2O  and  HCl+Aq.  (Godef- 
froy,  B.  8.  9.) 

+2H2O.  Sol.  in  H2O.  (Wyrouboff,  J.  B. 
1887.  538.) 

Cuprous  sodium  chloride. 
Very  sol.  in  H2O. 


302 


CUPRIC  SODIUM  CHLORIDE 


Cupric  sodium  chloride. 

Easily  sol.  in  cone.  NaCl-f-Aq.  Sol.  in 
alcohol  of  0.837  sp.  gr. 

No  double  salt  exists.  (Schreinemakers 
and  de  Baat,  Z.  phys.  Ch.  1909,  66.  586.) 

Cupric  thallic  chloride,  CuCl2,  2T1C13. 
Sol.  in  H2O.    (Willm,  A.  ch.  (4)  6.  55.) 
+6H2O.     Can   be   cryst.   from   H2O. 

(Gewecke,  A.  1909,  366.  225.) 

Cuprous   chloride   ammonia,   Cu2Cl2,    NH3. 

(Lloyd,  J.  phys.  Chem.  1908,  12.  399.) 

Cu2Cl2,  2NH3.  Decomp.  by  H2O  or  acids, 
not  by  alcohol.  (Ritthausen,  J.  pr.  59.  369.) 

Cu2Cl2,  3NH3.  (Lloyd,  J.  phys.  Chem. 
1908,  12.  399.) 

Cu2Cl2, 6NH3.  (Lloyd,  J.  phys.  Chem.  1908, 
12.  399.) 

Cupric  chloride  ammonia,  CuCl2,  2NH3. 
Decomp.  by  H2O.    (Kane,  A.  ch.  72.  273.) 
CuCl2,4NH8.    Sol.inH2O.    (Bouzat,C.R. 

1902,  135.  294.) 

+H2O  (Cuprammonium  chloride).  Sol. 
in  H2O  and  hot  NH4OH+Aq. 

+2H2O.  Sol.  in  small  amt.  of  H2O. 
Cu(OH)2  is  pptd.  by  dilution.  (Bouzat, 
A.  ch.  1903,  (7)  29.  350.) 

CuCl2,  5NH3.  (Bouzat,  A.  ch.  1903,  (7)  29. 
350.) 

+  1^H2O.  Sol.  in  H20.  On  dilution 
Cu(OH)2  is  pptd.  Sol.  in  NH4OH+Aq; 
solubility  decreases  as  NH3  concentration 
increases.  (Bouzat,  A.  ch.  1903,  (7)  29.  350.) 

CuCl2,  6NH3.  Completely  sol.  in  H2O. 
(Rose,  Pogg.  20.  55.) 

Sol.  in  H2O  but  decomp.  by  great  dilution 
with  pptn.  of  Cu(OH)2. 

Insol.   in  liquid   NH3.      (Bouzat.   A.    cb. 

1903,  (7)  29.  350.) 

Cuprocupric  chloride  ammonia,  Cu2Cl2,  CuCl2, 

Decomp.  by  H2O  or  alcohol.  Abundantly 
sol.  in  NH4Cl+Aq,  but  with  partial  decom- 
position. (Ritthausen.) 

Cupric  chloride  ammonia  platinous  chloride, 

CuCl2,  4NH3,  PtCls. 
See  Platodiamine  cupric  chloride. 

Cuprous  chloride  carbon  monoxide, 
Cu2Cl2,  2CO+4H2O. 

Very  sol.  in  HC1  (sp.  gr.  1.19)  with  evolu- 
tion of  CO.  Sol.  in  NH4OH-f  Aq.  (Man- 
chot  and  Friend,  A.  1908,  359.  110.) 

2Cu2Cl2,  CO+2H2O.  Insol.  in  H2O.  (Ber- 
thelot,  A.  ch.  1856,  (3)  46.  488.) 

4Cu2Cl2,3CO+7H2O.  Insol.  in  H20, 
but  decomp.  therewith  very  quickly.  Sol. 
in  Cu2Cl2+HCl. 


Cupric   chloride   hydrazine,   CuCl2,   2N2H4. 
Easily  decomp.     (Hofmann  and  Marburg, 
A.  1899,  305.  222.) 

Cuprous  chloride  mercuric  sulphide,  Cu2Cl2) 

2HgS. 

Insol.  in  H2O;  sol.  in  cone,  hot  HCl+Aq; 
not  decomp.  by  boiling  dil.  H2SO4+Aq,  but 
decomp.  by  cone.  H2SO4.  (Heumann,  B.  7. 
1390.) 

Cuprous  fluoride,  Cu2F2. 

Insol.  in  H20  or  HF.  Sol.  in  cone.  HCl-f 
Aq,  from  which  it  is  precipitated  by  H2O. 
Insol.  in  alcohol.  (Berzelius,  Pogg.  1.  28.) 

Decomp.  by  H2O  into  sol.  CuF2.  Sol.  in 
boiling  HCl+Aq  and  in  HNO3+Aq.  Only 
si.  attacked  by  warm  H2SO4.  (Poulenc,  C.  R. 
116.  1447.) 

Cupric  fluoride,  CuF2. 

Easily  takes  up  H2O  to  form  CuF2+2H2O. 
Sol.  in  HC1,  HNO3,  or  HF+Aq.  (Poulenc,  C. 
R.  116.  1448.) 

Solubility  at  25°  in  HF-f  Aq. 


Normality  of  HF  +Aq. 

g.  atoms  Cu  in  1000  c.  c. 
of  solution 

0.12 
0.28 
0.57 
1.08 

2.28 

0.0307 
0.1164 
0.2494 
0.388 
0.463 

Solubility  is  decreased  by  presence  of  KF. 
(Jaeger,  Z.  anorg.  1901,  27.  29.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  827.) 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 

+2H2O.  SI.  sol.  in  cold,  decomp.  by  hot 
H2O.  (Berzelius.) 

Cupric  hydrogen  fluoride,  CuF2,  5HF+5H2O. 

Deliquescent. 

Easily  sol.  in  H2O  and  dil.  acids. 

Sol.  in  NH4OH+Aq  with  decomp.  (Bb'hm, 
Z.  anorg.  1905,  43,  329.) 

Cupric  potassium  fluoride,  CuF2,  2KF. 

Easily  sol.  in  H20. 

CuF2,  KF.  Very  si.  sol.  in  H2O;  si.  sol.  in 
dil.  acids.  (Helmholt,  Z.  anorg.  3.  115.) 

Cupric  rubidium  fluoride,  CuF2,  RbF. 
As  the  K  salt.    (Helmholt.) 

Cupric  silicon  fluoride. 
See  Fluosilicate,  cupric. 


CUPRIC  HYDROXIDE 


303 


Copper  stannic  fluoride. 
See  Fluostannate,  copper. 

Copper  tantalum  fluoride. 
See  Fluotantalate,  copper. 

Copper  titanium  fluoride. 
See  Fluotitanate,  copper. 

Copper  tungstyl  fluoride. 
See  Fluoxytungstate,  copper. 

Copper  zirconium  fluoride. 
See  Fluozirconate,  copper. 

Cupric    fluoride    ammonia,    CuF2,    4NH3  + 
5H2O. 
Decomp.  rapidly  in  the  air. 
Easily  sol.  in  H2O. 
Decomp.  by  boiling  with  H20  with  evolu- 
tion of  NH3. 
Easily  sol.  in  dil.  acids.    (Bohm.  Z.  anorg. 
1905,  43.  333.) 

SolubiUty  in  NH4OH+Aq  at  25°. 

NHs  nc  nr>. 

g.  Cu  per  1. 

equiv.  CuOzHz 
perl. 

2.63 
2.00 
1.32 

3.05 
2.12 
1.08 

0.096 
0.067 
0.034 

2.540 
1.965 
1.280 
0.973 
0.870 
0.540 
0.391 

6.26 
6.28 
4.13 
3.36 
3.08 
2.36 
2.04 

0.197 
0.166 
0.129 
0.106 
0.097 
0.074 
0.064 

3.176 
2.070 
1.272 
0.451 
0.320 

8.06 
5.72 
4.75 
2.54 
2.13 

0.253 
0.180 
0.149 
0.080 
0.067 

The  non-agreement  of  the  results  is  due  to 
the   presence   of   different   modifications   of 
CuO2H2. 

Cuprous  hydride,  CuH. 

Insol.  inH20.  Sol.  in  HCl+Aq.  (Wurtz, 
C.  R.  18.  102.) 

Sol.  in  warm  cone.  HC1  with  decomp. 
(Bartlett,  Am.  Ch.  J.  1895,  17.  187.) 

Cupric  hydride,  CuH2. 

Sol.  in  HC1  with  decomp.  (Bartlett,  Am. 
Ch.  J.  1895,  17.  187.) 

Copper  hydrosulphide,  7CuS,  H2S. 

(Linder  and  Picton,  Chem.  Soc.  1892,  61. 

120.) 

9CuS,  H2S.    (Linder  and  Picton.) 
22CuS,  H2S.    (Linder  and  Picton.) 

Cuprous  hydroxide,  Cu2O,  zH2O. 

Sol.  in  acids  as  cupric  salt.  Insol.  in  NaOH, 
or  KOH+Aq. 

Sol.  in  NH4OH,  and  (NH4)2CO3+Aq;  sol. 
in  Na2S2O3+Aq. 

Cuprocupric   hydroxide,    CuOH,    3Cu(OH)2 

+3H2O. 
Sol.  in  acids.    (Francke,  Dissert.  1907.) 

Cupric  hydroxide,  3CuO,  H2O. 

Insol.  in  H2O  or  dil.  alkalies.  Easily  sol. 
in  warm  NH4Cl+Aq.  (Rose.) 

Much  more  difficultly  sol.  than  Cu02H2  in 
KOH+Aq.  (Chodnew,  J.  pr.  28.  220.) 

True  composition  is  6CuO,  H2O. 

See  also  Cupric  oxide. 

CuO2H2.  Insol.  in  H2O,  but  decomp.  into 
6CuO,  H2O  by  being  boiled  therewith. 

Extremely  easily  sol.  in  acids. 

Sol.  in  NH4OH,  and  NH4  salts  +  Aq. 


.(Bonsdorff,  Z.  anorg.  1904,  41.  182.) 
Solubility  in  NH4OH+Aq  at  18°. 


NHs  mols  per  1. 

Cu  g.  atoms  per  1. 

0.20 

0.00054 

0.50 

0.0033 

1.0        * 

0.0109 

1.5 

0.0204 

2.0 

0.0314 

2.5 

0.0442 

3.0 

0.0548 

4.0 

0.0784 

5.0 

0.  1041 

6.0 

0.1254 

8.0 

0.1599 

9.96 

0.1787 

(Dawson,  Z.  phys.  Ch.  1909,  69.  111.) 

Sol.  in  cold  NaOH,  or  KOH+Aq  (Proust); 
but  CuO  is  pptd.  on  boiling  (Berthollet) :  is 
not  pptd.  (Chodnew,  J.  pr.  28.  220.) 

Insol.  in  NaOH  or  KOH+Aq  unless  they 
contain  organic  matter  (Berzelius).  This  is 
contradicted  by  Volcker  (A.  59.  34). 

Entirely  sol.  in  cone.  KOH+Aq,  but  solu- 
tion is  decomp.  by  heating.  (Tremy,  A.  ch. 
(3)  12.  510.) 

Sol.  in  NaOH+Aq  (70%  NaOH).  (Low, 
Z.  anal.  9.  463.) 

The  solubility  in  NaOH  of  CuO2H2,  pre- 
pared either  from  CuSO4  or  Cu(NO3)2,  de- 
creases with  decrease  in  concentration  of  the 

3e.  The  solubility  of  CuO2H2  in  NaOH 
is  only  very  slightly  affected  by  the  addition 
of  sodium  or  potassium  carbonate.  (Fischer, 
Z.  anorg.  1904,  40.  41.) 


304 


CUPRIC  HYDROXIDE 


Solubility  of  crystalline  CuO2H2  in  ammoni- 
acal  Ba(OH)2  and  NaOH  solutions  at 

Solubility  of  crystalline  Cu02H2  in  ammoni- 
acal  salt  solutions  at  18°  —  Continued 

18°. 

Cone,  of  dis- 

Cu concentra- 

Solvent contains  per  litre 

solved  Cu.  g. 

Solvent  contains  per  litre 

tion  g.  atoms 

atoms  per  1. 

per  1. 

3  mol.  NH3+0.10  mol.  (NH4)2SO4 
"              +0.20 

0.1740 

1  mol.   NH3+0       mol.  Ba(OH)2 

0.01090 

+0.0025 

0.00907 

+0.40 

0   ^044- 

+0.005 

0.00801 

4  mol.  NHs+0.00  mol.  (NH4)2SO4 

\J  .  UU^ETc 

0.0784 

"        +0.01            " 

0.00633 

+0.01 

0  OQ22 

+0.02 

0.00526 

"              +0.025 

\j  .  \*<j£*j 
01  101 

2  mols.  NH3+0       mol.  Ba(OH)2 

0.0314 

+0.05 

.  11U1 

0  13Q7 

"         +0.01            " 

0.0277 

"              +0.10               " 

\J  .   XOi7  i 

0  9009 

4  mols.  NH3+0       mol.  Ba(OH)2 

0.0784 

+0.20 

OS  100 

+0.01 

0.0747 

"              +0.40                " 

.  OXoo 

0  5451 

1  mol.  NH3+0       mol.  NaOH 

0.0109 

5  mol.  NHa+0.00  mol.  (NH4)2SO4 

o!l041 

"        +0.01            " 

0.00766 

+0.01 

0.  1154 

"         +0.02            " 

0.00655 

+0.025 

0  1*320 

"         +0.03            " 

0.00531 

"              +0.05 

\J  .  XO^vf 

"         +0.05            " 

0.00456 

"          +0.10           MV 

O99QQ 

+0.10 

0.00410 

+0.20 

0^3415 

(Dawson,  Chem.  Soc.  1909,  96.  377.) 

"              +0.40 
1  mol.  NHs+0.00  mol.  Na2SO4 

0.5615 
0.0109 

Solubility  of  crystalline  CuO2H2  in  ammoni- 

+0.025 

0.0134 

acal  salt  solutions  at  18°. 

+0.10 
"              +0  20                " 

0.0162 

Of\~i  r*o 

Cone,  of  dis- 

"             +0.40               " 

.0192 

0   O7ft4. 

Solvent  contains  per  litre 

solved  Cu.  g. 
atoms  per  1. 

4  mol.  NHs+0.10  mol.  Na2SO4 

0.0994 

+0.20               " 

01  ifii 

1    w*sO     "\TTT« 

0  01  OQ 

.  11D1 

1   IllOl,   JNilS 

0.05  mol.  NHs+O.OI  mol.  (NH4)2SO4 

ol  00129 

(Dawson,  Chem.  Soc.  1909,  95.  373.) 

+0.025 

0.00511 

0.1    mol.  NHs+0.01  mol.  (NH4)2SO4 

0.00326 

+0.025 
+0.05 
0.2    mol.  NHs+0.00  mol.  (NH4)2SO4 
+0.01 
+0.025 
+0.05 
+0.10 
0.5    mol.  NHs+0.00  mol.  (NH4)2SO4 

"                      i  n    ni                      " 

0.0108 
0.0233 
0.00054 
0.00649 
0.0175 
0.0384 
0.0690 
0.0033 
00197 

SI.  sol.  in  alkali  carbonates  +Aq,  especially 
KHCO3  and  NaHCO3.    (Berzelius.) 
Sol.  in  cold  Na2S2O3+Aq,  but  ppfcd.  on 
warming.    (Field,  Chem.  Soc.  (2)  1.  28.) 
Partially  sol.  when  freshly  pptd.  in  KCN 
+Aq.     (Rodgers,  1834.) 
Sol.  in  (NH4)2S2O8+Aq.    (Moreau,  Apoth. 
Ztg.  1901,  16.  383.) 

-f-U.  Ul 
+0.025 
•<              +0.05               " 

.  U  J  _  / 

0.0284 
0  0536 

Sol.  in  MSCN+Aq.;  more  difficultly  sol. 
in    NH4SCN+Aq    than    ZnO2H2.      (Gross- 

+0.10 
+0.20 
1.0    mol.  NHs+0.00  mol.  (NH4)2SO4 
+0.01 

oiiois 

0.1844 
0.0109 
0.0210 

mann,  Z.  anorg.  1908,  58.  269.) 
Very   sol.   in  hydroxylamine.      (Jannasch 
and  Cohen,  J.  pr.  1905,  (2),  72.  14.) 
Insol.  in  acetone.    (Eidmann,  C.  C.  1899. 
II.  1014.) 

+0.05 
**                _LA   in                 ** 

0!0660 

Sol.  in  large  amt.  in  NaC2H302  +Aq.    (Mer- 
cer, 1844.) 

-j~U  .  1U 
+0.20 

0^2275 

Not  pptd.  in  presence  of  Na  citrate.    (Spil- 

+0.40 
2        mol.  NHs+0.00  mol.  (NH4)2SO4 
+0.01 
+0.025 
+0.05 
"              +0.10               " 

0.4135 
0.0314 
0.0462 
0.0605 
0.0886 
0.1468 

ler.) 
Insol.  in  cane  sugar  +Aq,  unless  an  alkali  or 
alkaline  earth  is  present.    (Peschier.) 
Recently  pptd.  CuO2H2  is  easily  sol.  in  cane 
sugar  with  NaOH,  KOH,  or  CaO2H2+Aq; 
[ess  sol.  in  presence  of  SrO2H2  or  Ba02H2. 

+0.20 
+0.40 

0.2591 
0.4718 

(Becquerel.) 
Not  pptd.  by  KOH+Aq  in  solutions  con- 

3       mol.  NHs+0.00  mol.  (NH4)2SO4 
+0.01 
+0.025 
+0.05 

0.0548 
0.0672 
0.0847 
0.1156 

taining  tartaric  acid,  cane  sugar,  and  many 
other  non-volatile  organic  substances. 
Sol.  in  Ca,  Ba,  Sr,  K  or  Na  sucrates+Aq, 
and  ppts.  of  double  sucrates  form  when  solu- 
tions of  the  first  three  bases  are  heated,  but  no 

CUPROUS  IODIDE 


305 


ppt.  fonns  in  the  last  two  cases  even  at  100°. 

Solubility  of  Cu2I2  in  I2+Aq  at  20°. 

Insol.  in  simple  Ca,  Ba,  or  K  su  crates  +Aq, 

!••                   i  "      j     1               ll'                                                *» 

g.  per  1. 

but  immediately  sol.  when  an  excess  of  cane 

Solid  Phase 

sugar  +Aq  is  present.    (Peligot.) 
Moderately  sol.  in  amyl  amine,  easily  sol.  in 
methyl,  less  in  ethyl  amine.     (Wurtz.) 
Sol.  in  sorbine+Aq.    (Pelouze.) 

0.285 
0.482 
0  583 

0.585 
1.305 

1    Q9*> 

Cu2I2 

Not  pptd.  in  presence  of  aromatic  oyxacids 
or  phenols  of  the  ortho  series.    Thus  in  pres- 

0^678 
0  756 

i  .  .  '—  -- 

2.557 
3  204 

ence  of  salicylic   acid,   pyrocatechin,   gallic 
acid,  pyrogallic  acid,  etc.,  NaOH+Aq  does 
not  ppt.   CuO2H2  from   Cu   solutions,   but 

(K844 

0.898 
0.964 

3^954 
4.436 

pptn.  is  not  prevented  by  benzoic  acid,  re- 

1  032 

5.685 

sorcin,    hydroquinone,    etc.     (Weith,    B.    9. 

1.090 

6^282 

342.) 
Sol.  in  solutions  of  alkali  salts  of  "spal- 
tungsprodukte"    of   albumen.      (Kalle   and 

1.112 
1.232 
i    f)40 

6.530 
7.653 
fi  44Q 

Cu2I  +I2 

Co,  Pat.  1901.) 

X  .  V_T±VJ 

0  808 

U  .  rir±t7 

^   «iQ4 

2 

Sol.  in  starch  emulsion  which  has  become 

\J  .  Oi/O 

0.748 

iJ  .  Uty^t 

4.711 

thin  liquid  in  an  alternating  magnetic  field. 

0.606 

3  856 

(Rosenthal,  C.  C.  1908,  1.  593.) 
CuO,  2H2O.     (Rubenovitch,  C.  R.  1899, 

0^448 
0.300 

2  '949 
2.069 

129.  336.) 

0  159 

1    230 

CuO,  3H2O.     CKosmann,  Z.  anorg.  1893, 
3.  373.) 

0^925* 

J  .  -£OU 

5.461 
US66 

Cu2I2+I2 

2CuO,  3H2O.    (Cross,  Gm—  K.  5.  1,  753.) 

' 

.  ouu 

4CuO,    H2O.      Insol.    in    NH4OH+Aq. 

*  at  0°.    **  at  40°. 

(Mailhe,  A.  ch.  1902,  (7)  27.  393.) 

(Fedotieff,  Z.  anorg.  1911,  69.  26.) 

Cupric  hydroxide  ammonia,  Cu02H2,  4NHs. 
Present  in  ammoniacal  solution  of  CuO2H2. 
(Dawson,  Z.  phys.  Ch.  1909,  69.  110.) 

Cuprous  imide,  Cu2NH. 

Decomp.  at  160°  forming  Cu3N. 

Readily  hydrolysed  by  H2O. 

Sol.  in  liquid  NH3  solutions  of  NH4N08. 
(Franklin,  J.  Am.  Chem.  Soc.  1912,  34.  1502.) 

Cuprous  iodide,  Cu2I2. 

Insol.    in  H2O,  or  dil.  acids. 

Calculated  from  electrical  conductivity  of 
Cu2I2+Aq,  1  1.  H2O  dissolves  about  8  mg. 
Cu2I2  at  18°.  (Kohlrausch  and  Rose,  Z.  phys. 
Ch.  12.  241.) 

Sol.  in  cone.  H2SO4.  (Vitali,  Gm.— K. 
6.  1,  947.) 

Sol.  with  difficulty  in  cone.  HCl+Aq. 

Decomp.  by  cone.  HNO3,  or  H2SO4.  Insol. 
in  NaCl,  KNO3,  Na2SO3,  KBr,  or  NH4C1+ 
Aq.  Sol.inNH4OH,Na2S203,KCN,orKI  + 
Aq.  (Renault,  C.  R.  59.  558.) 

Appreciably  sol.  in  N/10  HC1.  Practically 
insol.  in  N/10  H2SO4.  (Moser,  Z.  anal.  1904, 
43.  604.) 

Results  of  experiments  on  solubility  of 
Cu2l2  in  I2+Aq  in  presence  of  acids  and 
salts  are  given  by  Bray  and  MacKay. 

Cu2I2  was  found  to  be  si.. sol.  in  H2O  but 
a  considerable  amt.  dissolves  in  presence  of 
I2,  owing  to  formation  of  Culo  and  Culs-  (J. 
Am.  Chem.  Soc.  1910,  32.  1207.) 


Solubility  in  NH4Br+Aq  at  20°. 


NEUBr+Aq. 

g.  Cu2lz  in  1  1.  of  the 
solution 

2-N 
3-N 

4-N 

1.9068 
3.6540 
6.0588 

(Kohn  and  Klein,  Z.  anorg.  1912,  77.  254.) 

Sol.  in  FeCl3+Aq.    (Fleischer,  C.  N.  1869, 
19.  206.) 

Solubility  in  KBr+Aq  at  t°. 


t° 

KBr+Aq. 

g.  Cuzl2  in  1  I.  of 
the  solution 

19.5 
24.0 
19.5 
23.0 
22.0 
22.0 

2-N 
2-N 
3-N 
3-N 

4-N 
4-N 

1.4666 
1.5576 
3.4094 
3.5949 
7.1263 
6.9768 

The  solutions  undergo  change  in  the  course 
of  a  few  days,  iodine  being  set  free;  the  sol- 
ubility of  the  cuprous  iodide  is  not  markedly 
affected  thereby. 

(Kohn,  Z.  anorg.  1909,  63.  337.) 

1  1.  of  a  0.2N  solution  of  KI  dissolves 
0.000157  g.  mol.  Cu2I2.  (Bodlander,  Z. 
anorg.  1902,  31.  475.) 

Very  sol.  in  liquid  NH8.  (Franklin,  Am. 
Ch.  J.  1898,  20.  827.) 


306 


CUPRIC  IODIDE 


Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.  257.) 

Practically  insol.  in  methvlene  iodide. 
(Retgers,  Z.  anorg.  1893,  3.  347.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Insol.  in  acetone  (Naumann,  B.  1904, 
37.  4329);  (Eidmann,  C.  C.  1899,  II,  1014.) 

100  g.  acetonitrile  dissolve  3.52  g.  Cu2I2 
at  18°.  (Naumann  and  Schier,  B.  1914,  47. 
249.) 

Mm.  Marshite.    (Gin— K.  5.  1,  945.) 


Cupric  iodide,  CuI2, 

Exists  only  in  very  dil.  aqueous  solution. 
(Traube,  B.  17.  1064.) 

Copper  periodide,  CuI4. 

Sol.  in  H2O.  (Walker  and  Dover,  Chem. 
Soc.  1905,  87.  1588.) 

Copper  ammonium  iodide  ammonia. 
See  Cupriammonium  iodide  ammonia. 

Cuprous  mercuric  iodide,  Cu2l2,  HgI2. 
KI+Aq  dissolves  out  BTgI2. 

Cuprous   mercuric   iodide   ammonia,    CuI2, 
2HgI2,  4NH3. 

Decomp.  by  H20  or  acids.  Sol.  in  a  mix- 
ture of  acetic  acid  and  alcohol. 

CuI2,  HgI2,  4NH3.  As  above.  (Jorgensen, 
J.  pr.  (2)  2.  347.) 

Cupric  nitrogen  iodide,  CuI2,  N2H4I2. 

Decomp.  by  H2O;  or  NH4OH+Aq.  (Guy- 
ard,  C.  R.  97.  526.) 

Cupric  thallic  iodide  ammonia,  CuI2,  2T1I3, 

4NH8. 

Decomp.  slowly  by  H2O.  Sol.inNH4OH+ 
Aq  with  decomp.  Sol.  in  alcohol. 

Cuprous  iodide  ammonia,  Cu2I2,  NH8. 

Ppt.  (Anderline,  Gazz.  ch.  it.  1912,  42.  I, 
321.) 

+4H2O.  Insol.  in  H2O.  Very  sol.  in 
NH4OH+Aq.  (Silberrad,  Chem.  Soc.  1905, 
87.  67.) 

Cu2I2,  3NH3.  (Lloyd,  J.  phys.  Chem. 
1908,12.399.) 

Cu2I2,  4NH3.    (Levol,  J.  Pharm.  4.  32S.) 

+H2O.     (Saglier,  C.  R.  104.  1440.) 

Cu2I2,  6NH8.    (Lloyd.) 

Cupric  iodide  ammonia,  CuI2,  4NH3+H2O. 

Decomp.  by  H2O.  Sol.in  NH4OH+Aq 
without  decomp.  Not  attacked  by  cold 


alcohol  or  ether.  (Berthemont,  J..  Pharm. 
15.  445.)  (Pozzi-Escot,  C.  R,  1900,  130.  90.) 

CuI2,  6NH3.  Sol.  in  liquid  NH3.  (Horn, 
Am.  Ch.  J.  1908,  39.  205.) 

3CuI2,  10NH3.  Decomp.  by  H2O.  (Rich- 
ards, Am.  Ch.  J.  1895,  17.  302.) 

Sol.  in  liq.  NH3.  (Horn,  Am.  Ch.  J.  1908, 
39.  204.) 

Cupriammonium   iodide    ammonia, 

3Cu(NH3)2I2,  4NH3. 

Decomp.  by  air  and  by  H2O.  (Richards, 
Am.  Ch.  J.  1895,  17.  302. 

Copper  periodide  ammonia,  2CuI,  I4,  5NH3 

+HaO. 

Because  of  its  insolubility  it  cannot  be 
recryst  from  any  solvent.  (Silberrad,  Chem. 
Soc.  1905,  87.  66.) 

Copper  tetraiodide,  ammonia,  CuI4,  4NH3. 
(Jorgensen,  J.  pr.  (2)  2.  353.) 

Copper  Aezaiodide  ammonia,  Cule,  4NH3. 

Not  decomp.  in  H2O  in  closed  vessels. 
(Jorgensen.) 

Copper    mercuric    iodide    ammonia, 
CuHg3I6,  5NH3. 

CuHgI3,  2NH3.  Ppt.  Decomp.  by  H2O 
and  by  alcohol. 

CuHg2I6,  3NH3.  Ppt.  Decomp.  by  long 
washing  with  H2O. 

CuHg2I5,  4NH3.  Ppt.  Decomp.  by  H2O. 
SI.  attacked  by  abs.  alcohol. 

CuI2,  HgI2,  4NH3.  Ppt.  (Anderline,  Gazz. 
ch.  it.  1912,  42,  (1)  321;  C.  C.  1912,  II.  95.) 

Copper  nitride,  Cu6N2. 

Decomp.  by  dil.  or  cone,  acids. 

Easily  decomp.  by  H2O  when  finely  pow- 
dered. (Rossel,  C.  R.  1895,  121.  942.) 


Copper  sw&oxide, 

Not  attacked  by  H2O.  Decomp.  by  dil. 
H2Sq4+Aq  into  Cu  and  CuSO4;  dil.  HCl+Aq 
has  similar  action.  Not  attacked  by  NH4OH 
+Aq  or  NH4OH+(NH4)2CO8+Aq.  (Rose, 
Pogg.  120.  1.) 

Cu3O.  Not  attacked  by  dil.  or  cone.  min. 
acids,  even  aqua  regia.  Slowly  sol.  in  HF-f- 
Aq.  (Bailey  and  Hopkins,  Chem.  Soc.  1890, 
67.  272.) 

Is  a  solution  of  oxide  in  Cu.  (Jordis, 
Zeit.  angew.  Ch.  1908,  21.  51.) 

Cuprous  oxide,  Cu2O. 

Insol.  in  H2Q.  Decomp.  by  H2SO4+Aq, 
H3PO4+Aq,  or  cold  very  dil.  HNO3+Aq  into 
a  cupric  salt  and  Cu.  Converted  by  HC1+ 
Aq  into  cuprous  chloride. 


CUPRIC  OXIDE 


307 


Solubility  of  Cu2O  in  NH4OH+Aq  at  25°. 

Solubility  of  CuO  in  HF+Aq  at  25°. 

Cone,  of  total  Cu 

Cone,  of  total  NH3 

Time 

G.  CuO  in  10  ccm. 
of  the  solution 

G.  in  1000  g. 
of  solution 

G.  mol.  in 
1000  g.  of 
solution 

G.  in  1000  g. 
of  solution 

G.  mol.  in 
1000  g.  of 
solution 

0.25N-H* 

Ikhrs. 

25k  ;; 

17Q1A    " 

0.0431 
0.0619 
0.0812 
0.0823 
0.0907 

Preparation  I 

0.3593 
0.5024 
0.6869 
0.6964 
1.0144 
1.0462 
1.0557 
1.2243 
1.3229 
1.4882 
1.5105 
1.6313 
1.6981 

0.00566 
0.00791 
0.01080 
0.01095 
0.01597 
0.01645 
0.01660 
0.01924 
0.02081 
0.02340 
0.02375 
0.02565 
0.02670 

3.91 
12.07 
13.77 
16.15 
27.03 
32.64 
36.89 
45.73 
68.68 
74.12 
81.26 
98.52 
122.40 

0.23 
0.71 
0.81 
0.95 
1.59 
1.92 
2.17 
2.69 
4.04 
4.36 
4.78 
5.56 
7.20 

N-HF  (a) 

52  2    " 
201^    " 
226^    " 

0.3018 
0.2797 
0.2747 
0.2339 
0.2353 

N-HF  (b) 

4k    " 
44k    " 

117%  ;; 

0.3220 
0.2930 
0.2431 
0.2219 

2.02N-HF 

5  *    1' 
156^1    " 

0.3646 
0.4533 
0.3583 
0.3311 

Preparation  II 

(Deussen,  Z.  anorg.  1905,  44.  421.) 

Solubility  of  CuO  in  HF  at  25°. 
Cu  =  g-atoms  Cu  in  1  1.  of  the  solution. 

0.4229 
0.6678 
0.9890 
1.0494 
1.3528 
1.5047 
1.5963 
1.6555 

0.00665 
0.01050 
0.01555 
0.01650 
0.02127 
0.02366 
0.02510 
0.02603 

7.82 
8.16 
22.61 
28.39 
54.15 
72.08 
78.20 
102.05 

0.46 
0.48 
1.33 
1.67 
3.19 
4.24 
4.60 
6.00 

HF  normality                                    Cu 

0.12                              0.0307 
0.28                             0.1164 
0.57                             0.2494 
1.08                             0.388 
2.28                             0.463 

(Donnan  and  Thomas,  Chem.  Soc.  1911,  99. 
1791.) 

Sol.  in  boiling  NH4Cl+Aq.    (Rose.) 

SI.  sol.  in  excess  of  KOH  +  Aq .    (Chodnew.) 

Sol.    in    cone.    MgCl2,    and    FeCl2-fAq. 

(Hunt,  C.  R.  69.  1357.) 
SI.  attacked  by  liquid  NH3.     (Gore,  Am. 

Ch.  J.  1898,  20.  827.) 

Min.  Cuprite.     Sol.  in  HC1,  HN03,  and 

NH4OH+Aq. 

Cupric  oxide,  CuO. 

Insol.  in  F2O.  Easily  sol.  in  acids.  Sol. 
in  H2SO3+Aq.  Insol.  in  NH4OH+Aq,  but 
dissolves  on  addition  of  a  few  drops  of  acid 
or  (NH4)2CO3+Aq.  Insol.  in  dil.,  but  sol.  in 
warm  cone.  NaOH,  and  KOH+Aq.  (Low, 
Z.  anal.  9.  463.) 

CuO  prepared  at  a  low  temp,  is  easily  sol. 
in  dil.  acids,  but  when  ignited  is  slowly  sol. 
in  boiling  cone,  acids,  but  moderately  rapidly 
in  a  cold  mixture  of  NHJ+HC1.  (Joannis, 
C.  R.  1886,  102.  1161.) 

Solubility  in  N-HNO3.  1  1.  of  the  solution 
contains  0.4802  g.  atoms  Cu  at  25°.  (Jaeger, 
Z.  anorg.  1901,  27,  33.) 


(Jaeger,  Z.  anorg.  1901,  27.  29.) 

Solubility  of  CuO  in  HF+KF  at  25°. 
Cu  =  g-atoms  Cu  in  1  1.  of  the  solution. 


HF  normality 

Cu 

0.12 

0.28 
0.57 
1.  11(1.  08) 

2.17(2.28) 

0.0356 
0.06437 
0.1442 
0.2451 
0.2517 

(Jaeger,  1.  c.) 

SI.  sol.  in  large  excess  of  KOH+Aq.  (de 
Coninck,  C.  C.  1904,  II,  65.) 

Slowly  sol.  in  boiling  NH4Cl+Aq,  and 
less  easily  in  NH4NO3+Aq.  (Rose.) 

Sol.  in  boiling  H2O  solutions  of  A12,  Gl, 
U,  Cr2,  Fe2,  or  Bi  nitrates  and  chlorides, 
Hg(NO3)?,  Hg2(NO3)2,  SbCl3,  SnCl2,  and 
SnCl4,  with  pptn.  of  oxides  of  the  bases  of 
those  salts.  Unacted  upon  by  boiling  H2O 
solutions  of  Mn,  Mg.  Ni,  Co,  Zn,  Ce,  or 


308 


CUPROCUPRIC  OXIDE 


Fe  nitrates  or  chlorides,  AgNO3,  Pb(N03)2, 
Cd(NO3)2,  and  HgCl2.    (Persoz.) 

Pure  CuO  is  very  si.  sol.  in  NH4OH+Aq 
but  the  solution  is  greatly  increased  by  the 
addition  of  NH4  salts.  (Muthmann,  C.  C. 
1904.  II,  410.) 

Sol.  in  hot  (NH4)2SO4  or  (NH4)2S03+Aq. 
(Jumau,  Electrochem.  Ind.  1908,  6.  258.) 

15%  dissolves  in  (NH4)oCO3+Aq  in  '24 
hrs.  (Schnabel,  Z.  B.  H.  Sal.  1880,  28.  282.) 

SI.  attacked  by  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  827.) 

Solubility  in  N-acetic  acid.  1  1.  of  the  solu- 
tion contains  0.1677  g-atoms  Cu  at  25°. 
(Jaeger,  Z.  anorg.  1902,  27.  33.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

SI.  sol.  in  benzamide.  (Dessaignes,  A.  ch. 
1852,  (3),  34.  146.) 

Insol.  in  piperidine.  (Cahours,  G.  R. 
1852,  34.  481.) 

'  Sol.  in  acid  amines  as  asparagin.    (Piria, 
A.  ch.  1848,  (3),  22.  160.) 

Sol.  in  amines  alone  or  mixed  with  NH3. 
(Lance,  Dissert.  1906.) 

Slowly  sol.  in  Ca  or  any  other  alkali  su- 
crate+Aq,  but  not  in  cane  sugar +Aq. 
(Hunton.) 

Solubility  in  (calcium  su crate + sugar)  +Aq. 

1  1.  solution  containing  418.6  g.  sugar  and 
34.3  g.  Cap  dissolves  10.26  g.  CuO. 

1  1.  solution  containing  296.5  g.  sugar  and 
24.2  g.  CaO  dissolves  5.68  g.  CuO. 

1  1.  solution  containing  174.4  g.  sugar  and 
14.1  g.  CaO  dissolves  3.47  g.  CuO.  (Boden- 
bender,  J.  B.  1865.  600.) 

Polypeptides  in  aqueous  solution  dissolve 
CuO  by  short  boiling.  (Fischer,  B.  1906,  39. 
576.) 

+  V6H2O=6CuO+H2O.  Insol.  in  dil., 
but  sol.  in  cone.  KOH  or  NaOH  -fAq. 

Sol.  in  volatile  oils. 

See  also  Cupric  hydroxide. 

Min.  Melaconite.  Sol.  in  HC1,  or  HNO3  + 
Aq. 

Cuprocupric  oxide,  Cu5O3=2Cu2O,  CuO. 

(Favre  and  Maumene".) 

Cu3O2+H2O  =  Cu2O,  CuO+H2O.  When 
freshly  pptd.,  sol.  in  HCl+Aq,  but  insol.  after 
drying.  (Siewert,  J.  B.  1866.  257.) 

Cu4O3  =  Cu2O,  2CuO.     (Siewert.) 

All  oxides  of  Cu  except  Cu4O,  Cu2O,  CuO, 
and  CuO2  are  mixtures.  (Osborne,  Sill.  Am. 
J.  (3)  32.  33;  Debray,  C.  R.  99.  583.) 

Copper  dioxide,  CuO2+H2O. 

Insol.  in  H2O.  Decomp.  by  acids  with  for- 
mation of  cupric  salt  and  H2O2.  (Weltzien, 
A.  140.  207.) 

Cuprous  oxide  ammonia  (cuprosammonium 

oxide). 

Known  only  in  solution.  (Wagner,  C.  C. 
1863.  239.) 


Cupric  oxide  ammonia  (cuprammonium  hy- 
droxide), 3CuO,  4NH3+6H2O. 
Insol.  in  H2O.    (Kane,  A.  ch.  72.  283.) 
CuO,   4NF8+4H2O.     Very   deliquescent. 

Decomp.  in  the  air  and  by  H2O.    (Malaguti 

and  Sarzeau,  A.  ch.  (3)  9.  438.) 

Cuprous  oxybromide,  Cu2Br2,  CuO+H2O. 

(Spring  and  Lucion,  Bull.  Ac.  Bele;.  (3) 
24.  21.) 

Cupric  oxybromide,  CuBr2,  3CuO+3H2O. 

Insol.  in  H2O.  Easily  sol.  in  dil.  acids  or 
NH4OH+Aq.  (Brun,  C.  R.  109.  66.) 

Insol.  in  H2O  but  decomp.  by  continued 
boiling.  Sol.  in  cone,  acetic  acid,  si.  sol.  in 
cone.  CuBr2-fAq.  Insol.  in  dil.  KBr+Aq. 
(Richards,  Proc.  Am.  Acad.  1890,  25.  215.) 

Cupric  oxybromide  ammonia,  2CuO,  CuBr2, 

2NH3+3H2O. 

(Kohlschiitter  and  Pudschies,  B.  1904,  37. 
1159.) 

Cuprous  oxychloride,  Cu2Cl2,  CuO+3H20. 

(Spring  and  Lucion,  Bull.  Ac.  Belg.  (3) 
24.  21.) 

Cupric  oxychloride,  CuO,  CuCl2+H20. 

Decomp.  by  H2O.  (Rousseau,  C.  R.  1890, 
110.  1263.) 

2CuO,  CuCl2.  Insol.  in  H20.  Sol.  in  HC1 
4-Aq,  from  which  it  is  reprecipitated  by 
dilution  with  H2O. 

+H2O.    (Kane,  A.  ch.  72.  277.) 

+4H2O.    (Gladstone,  Chem.  Soc.  8.  211.) 

3CuO,  CuCl2+2H2O.  (Miller  and  Ken- 
rick,  Trans.  Roy.  Soc.  Can.  1901,  (2)  8,  III. 
35.) 

-j-3H2O.  (Dupont  and  Jansen,  Bull. 
Soc.  1893,  (3),  9.  193.) 

+33^H2O.  Insol.  in  cold  H2O,  si.  decomp. 
by  boiling.  (Reindel,  J.  pr.  106.  378.) 

Insol.  in  boiling  H2O.  (Habermann,  W.  A. 
B.  90.  2.  268.) 

+4H20.  Sol.  in  alkaline  solution  of  KNa 
tartrate.  (Groger,  Z.  anorg.  1902,  31.  327.) 

(Brunswick  green}.  Insol.  in  H2O.  Easily 
sol.  in  acids. 

Min.  Atacamite.  Sol.  in  acids,  and  NH4OH 
+Aq. 

Sol.  in  cold  sat.  citric  acid+Aq.  (Bolton, 
B.  1880,  13.  732.) 

4CuO,  CuCl2+6H2O.  (Kane,  Gm.— K. 
5.  1,  919.) 

+8H2O.  Min.  Tallingite.  (Church,  Gm. 
— K.  5.  1,  919.) 

5Cu(OH)o,  Cu,Cl2Cl(OH).  Insol.  in  H2O. 
Decomp.  by  hot  H2O.  (Kuhling,  B.  1901, 
34.  2852.) 

7CuO,   2CuCl2+9H2O.     (Reindel.) 

6CuO,CuCl2+9H2O.  Insol.  in  H2O.  Sol.  in 
acetic  acid.  (Neumann,  Repert,  37.  304.) 

8CuO,  CuCl2  +  12H2O.  Min.  Footeite. 
(Konig,  Zeit.  Kryst.  1891,  19.  601.) 


CUPROUS  SILICIDE 


309 


Cupric  zinc  oxychloride,  ZnO,  2ZnCl2,  5CuO 
+6H2O. 

(Andre,  C.  R.  1888,  106.  855.) 

Cupric  oxychloride  ammonia,  2CuO,  CuCl2, 

2NH3+3H20. 
(Deherain,  Gm.— K.  6.  1,  932.) 

Cupric  oxyfluoride,  CuO,  CuF2+H2O. 

InsDl.  in  H2O.  (Berzelius.)  (Balbiano, 
Gazz.  ch.  it.  14.  74.)  ' 

Cupric  oxyfluoride  ammonia  (cuprammonium 

oxyfluoride),  Cu(OH)F,  2NH3. 
(Balbiano,  Gazz.  ch.  it.  14.  74.) 
3CuO,  CuI2+zH2O.  (Tschiriwinski,  Gm. 

— K,  5.  1,  1584.) 

Cuprous  oxyiodide,  Cu2I2>  CuO  +H2O. 

(Spring  and  Lucion,  Bull.  Ac.  Belg.  (3) 

Cupric  oxyiodide,  2CuI2,  CuO+4H2O, 

Easily  decomp.  by  H2O.  (Carnegie,  Watts ' 
Diet.  II,  257.) 

Copper  oxysulphide,  2Cu2S,  CuO. 

Insol.  in  H2O.  (Maumene,  A.  ch.  (3)  18. 
311. 

5CuS,  CuO.  Ppt.  (Pelouze.) 

2CuS,  CuO.     Insol.  in  H2O. 

CuS,  CuO.    Insol.  in  H2O. 

Above  comps.  do  not  exist.  (Pickering, 
Chem.  Soc.  33.  136.) 

Copper  phosphide,  Cu6P2. 

Easily  sol.  in  HNO3  or  aqua  regia;  insol.  in 
HCl+Aq.  (Rose,  Pogg.  6.  209.) 

Sol.  in  HNO3  and  Br2+Aq.  Decomp.  by 
hot  cone.  H2SO4.  (Rubenovitch.  C.  R.  1899. 
128.  1399.) 

Cu2P.  Sol.  in  HNO3-f-Aq.  (Granger, 
A.  ch.  1898,  (7),  14.  64.) 

Crystallized.  Completely  sol.  in  hot  HN03, 
aqua  regia  and  HF+HNO3.  Slowly  sol.  in 
hot  HC1  or  H2SO4.  Not  attacked  by  hot  or 
cold  HF  or  acetic  acid.  (Maronneau,  C.  R. 
1899,  128.  939.) 

Cu3P2.  Easily  sol.  in  HNO3.  Sol.  in  hot 
cone.  H2SO4.  Sol.  in  cone.  HCl+Aq  before 
the  phosphide  has  been  heated.  (Rose.  Pogg. 
4.  110.) 

Cu2P2.  Easily  sol.  in  HNO3,  or  HCl+Aq. 
Sol.  in  NH4OH+Aq.  (Granger,  Bull.  Soc. 
(3)  9.  661.) 

CuP2.  Decomp.  by  HNO3;  not  readily 
sol.  in  HC1.  Easily  attacked  by  C12  or  Br4+ 
Aq.  (Granger,  C.  R.  1895,  120.  924.) 

Cu6P2.    (Granger,  C.  N.  1898,  77.  229.) 

Very  sol.  in  HNO3  and  Br2+Aq.  Decomp. 
by  hot  cone.  H2S04.  (Rubenovitch,  C.  R. 
1899,  129.  338.) 


Cupric  zinc  phosphide,  10Cu6P2,  Zn8P2(?). 
(Hvoslef,  A.  100.  99.) 

Copper  phosphoselenide,  CuSe,  P2Se. 

Insol.  in  H2O  or  HCl+Aq;  sol.  in  HNO3  + 
Aq.  Insol.  in  cold  alkalies,  but  decomp. 
slowly  when  heated  therewith.  (Hahn,  J. 
pr.  93.  436.) 

2CuSe,  P2Se3.  Attacked  only  by  fuming 
HN03.  (Hahn.) 

2CuSe,  P2Se6.  Sol.  only  in  HN03+Aq. 
(Hahn.) 

Copper  phosphosulphide,  2Cu2S,  P2S. 

Cu2S,  P2S.     (Berzelius.) 

2Cu,,S,  P2S3.    (Berzelius.) 

CuS,  P2S.  Insol.  in  H2O  and  dil.  HC1 
+Aq.  Sol.  in  cone.  HCl+Aq,  from  which  it 
is  precipitated  by  H2O.  (Berzelius,  A.  46. 
252.) 

8CuS,  P2S5.    (Berzelius.) 

Cu4PS3.  Sol.  in  cone.  HNO3  and  in  aqua 
regia.  Insol.  in  HC1.  Not  attacked  by  hot 
H2SO4  or  cone.  NaOH+Aq.  (Ferrand,  A 
ch.  1899,  (7),  17.  407.) 

Cuprous  selenide,  Cu2Se. 

Ppt.    Sol.  in  HC1  and  in  H2SO4. 

Decomp.  by  HNO3.  Sol.  in  NH4OH+Aq. 
(Fonzes-Diacon,  C.  R.  1900,  131.  1207.) 

Sol.  in  KCN+Aq.  (Heyn  and  Bauer, 
Metall.  1903,  3.  84.) 

Min.  Berzelianite. 

Cupric  selenide,  CuSe. 

(Little,  A.  112.  211.) 

Ppt.  Sol.  in  HC1  and  in  H2SO4.  Decomp. 
by  HNO3.  (Fonzes-Diacon,  C.  R.  1900,  131. 

Cuprocupric  selenide,  Cu3Se2. 

Min.  Umangite.  Sol.  in  HNO3.  (Klock- 
mann,  Zeit.  Kryst.  1891.  19,  270.) 

Cuprous  lead  selenide,  3Cu2Se,  PbSe. 

Min.  Zorgite.  Sol.  in  cold  cone.  HN03  + 
Aq  with  separation  of  Se. 

Cupric  lead  selenide,  CuSe,  PbSe. 

Sol.  in  cold  cone.  HNO3  with  separation  of 
Se.  (Karsten.) 

CuSe,  2PbSe.    As  above. 
CuSe,  4PbSe.     As  above. 

Cuprous  silver  selenide,  Cu2Se,  Ag2Se. 

Min.  Eucainite.  Sol.  in  hot  HN03  with 
decomp.  (Berzelius.) 

Cuprous  silicide,  Cu4Si. 

Sol.  in  warm  dil.  or  cone.  HNO3.  Only 
si.  sol.  in  HC1,  H2S04  and  HF.  Sol.  in  a 
mixture  of  HNO3  and  HF.  Not  attacked  by 
solutions  of  alkalies.  (Vi«;ouroux.  C.  R.  1906 
142.  88.) 


310 


CUPROUS  SULPHIDE 


Cu2Si3.  Sol.  in  aqua  regia  and  fused  sodium 
potassium  carbonate,  (de  Chalmot,  Am.  Ch. 
J.  1896,  18,  95.) 

Cu2Si.  Decomp.  by  water  and  moist  air, 
and  by  acids  and  fused  alkali.  (Vigouroux, 
C.  R.  1896,  122.  319.) 

Cuprous  sulphide,  Cu2S. 

More  sol.  in  H2O  than  Ag2S,  but  much  less 
than  PbS.  (Bodlander,  Z.  phys.  Ch.  1898. 
27,  64.) 

1  1.  H20  dissolves  3.1+1CH5  moles  Cu2S  at 
18°.  (Weigel,  Z.  phys.  Ch.  1907,  58.  294.) 

Very  slowly  decomp.  by  dil.  H2SO4  in 
presence  of  oxygen.  (Thompson,  Electro- 
chem,  Ind.  1904.  2,  225.) 

Decomp.  by  cone.  H2SO4.  (Pickering,  C.  N 
1878,  37,  37:) 

Cold  HNO3+Aq  dissolves  out  Cu  and 
leaves  CuS;  hot  HNQ2  dissolves  with  separa- 
tion of  S.  SI.  sol.  in  boiling  cone.  HC1  + 
Aq.  Insol.  in  (NH4)2S+Aq. 

5N-HC1  dissolves  Cu2S  very  slightly 
(0.0038  g.  Cu  in  7^  hrs.)  but  it  is  more  sol. 
in  presence  of  Cl,  when  0.672  g.  are  dis- 
solved in  7^2  hours.  (Egii,  Z.  anorg.  1902, 
30.  46.) 

Sol.  with  exclusion  of  air  in  NH4OH+Aq. 
(Malzac,  Pat.  1904.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Min.  Chalcocite.  Completely  sol.  in  warm 
HNO3  with  separation  of  S. 

Cupric  sulphide,  CuS. 

Almost  absolutely  insol.  in  H2O;  sol.  in 
950,000  pts.  H20.  When  exposed  to  the  air, 
dissolves  in  H2O  as  CuSO4.  Easily  sol.  in 
boiling  HNO3  with  separation  of  S.  Diffi- 
cultly sol.  in  hot  cone.  HCl+Aq.  Insol.  in 
dil.  H2SO4+Aq-(l:6).  (Hoffmann,  A.  115. 
286. 

Pptd.  by  H2S  or  (NH4)2S+Aq  in  presence 
of  100,000  pts.  H2O  (Pfaff),  200,000  pts.  H2O 
(Lassaigne),  15,000  pts.  H2O  and  7500  pts. 
HC1,  but  with  40,000  pts.  H2O  and  20,000 
pts.  HC1  no  colour  is  visible  (Reinsch). 

1  1.  H2O  dissolves  3.51  +  1(H  moles  CuS 
at  18°.  (Weigel,  Z.  phys.  Ch.  1907,  58.  294.) 

Insol.  in  H2SO3+Aq.  (Guerout,  C.  R. 
1872,  75.  1276.) 

Decomp.  by  cone.  H2SO4.  (Kliche,  J.  B. 
1890,  593.) 

Sol.in(NH4)2CO3+Aq.  (Berzelius.)  Sol. 
in  alkali  bicarbonates  +Aq. 

Insol.  in  NH4NO3.  or  NH4Cl+Aq.  (Brett.) 

Insol.  in  acidified  cone,  alkali  chlorides + 
Aq.  (Cushmann,  Am.  Ch.  J.  1895,  17,  382.) 

Sol.  in  FeCl3+Aq  with  separation  of  S. 
(Cumenge  and  Wimmer,  Dingl.  1883,  250. 
123.) 

Decomp.  by  boiling  CuCl2+Aq  in  presence 
of  HC1  or  NaCl.  (Raschig,  Gm— K.  5. 
1,  819.) 

Sol.  in  Fe2(SO4)3+Aq  in  presence  of  large 
excess  of  air.  (Thompson,  Electrochem. 
Ind.  1904,  2,  228.) 


Insol.  in  KOH,  or  K2S+Aq,  especially  if 
boiling;  appreciably  sol.  in  colourless  and 
even  more  readily  in  hot  yellow  (NH4)2S+Aq. 

SI.  sol.  in  Na2S+Aq,  more  easily  in  NaSH-f- 
Aq.  (Becker,  Sill.  Am.  J.  (3)  33.  199.) 

100  cc.  sat.  Na2S+Aq-(sp.  gr.  =  1.225) 
dissolve  0.0032  g.  CuS.  (Holland,  Ann. 
Chim.  Anal.  1897,"  2.  243.) 

Sol.  in  K  polysulphides  (3-64%).  (Prost, 
Bull.  Soc.  Belg.  Chim.  1897.  103.) 

Appreciably  sol.  in  alkali  polysulphides  + 
Aq.  •  (Rossing,  Z.  anal.  1902,  41,  1.) 

Sol.  in  considerable  quantity  in  alkali  sulph- 
arsenates,  sulphantimonates,  and  sulpho- 
stannates+Aq.  Therefore  when  a  mixed 
ppt.  of  CuS  and  As2S3,  Sb2S3,  or  SnS  is  treated 
with  K2S,  a  portion  of  the  CuS  is  dissolved. 
(Wohler,  A.  34.  236.) 

Sol.  in  alkali  sulphovandates,  or  sulpho- 
tungstates+Aq.  (Storch,  B.  16.  2015.) 

Sol.  in  alkali  sulphomolybdates  +  Aq. 
(Debray,  C.  R.  96.  1616.) 

Insof.  in  K  thiocarbonate  +  Aq.  (Rosen- 
bladt,  Z.  anal.  26.  15.) 

Sol.  inKCN+Aq. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790) ;  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Insol.  in  Na  xanthogenate.  (Ragg,  Ch. 
Z.  1908,  32.  677.) 

Solubility  of  CuS  in  sugar +Aq  at  t°. 
g.  CuS  per  1.  of  solution. 


t° 

10%  sugar 

30%  sugar 

50%  sugar 

17.5 
45 
75 

0.5672 
0.3659 
1  .  1345 

0.8632 
0.7220 
1.2033 

0.9076 
1  .  0589 
1.2809 

(Stolle,  Z.  Ver.  Zuckerind.  1900,  50.  331.) 

Min.  Covellite. 

Colloidal.  Aqueous  solution  is  stable  when 
it  contains  5  g.  CuS  in  a  litre;  when  it  contains 
4  or  5  times  that  amount  it  is  decomposed  in 
an  hour. 

Solutions  of  salts  of  the  following  concen- 
tration cause  a  precipitate  in  the  above  solu- 
tion. Salts  of  univalent  elements — 


Salts  of  univalent  elements — 

K3Fe(CN)6  1 

K4Fe(CN)6  1 

Na2S203  1 

Na2CO3  1 

Na2HP04  1 

Na2SO4  1 

K2Cr207  .    1 

KI  1 


KBr 
KClOa 


62 

127 

157 

200 

252 

333 

2083 

80 

133 

166 


CUPROUS  SODIUM  SULPHIDE 


311 


Salts  of  univalent  elements  —  Continued. 
NaCaH,O2                           1  :  221 
(NH4)2C2O4                        1  :  255 

Cupric  iron  (ferric)  sulphide,  CuS,  Fe2S8. 
Min.  Cubanite. 

NaCl    . 

1  :  400 

NaHCO3 

1  :  2500 

Copper  iron  potassium  sulphide,  K2FeCu«S4. 

K2S04  . 

1  :  117 

SI.  attacked  by  cold  dil.  HCl+Aq.     De- 

K2CrOi 
NaC7H502 

1  :133 
1  :  166 

comp.  by  warming.     (Schneider,  Pogg.  138. 
318.) 

K2S2O6        $* 

1  :222 

KC1      . 

.     1  :  333 

Copper  iron  sodium  sulphide,  Na2FeCu3S4. 

KNO3  . 

.     1  :  500 

Salts  of  bivalent  metals  — 

SI.  attacked  by  cold  dil.,  easily  decomp,  by 
hot  HCl+Aq.    (Schneider,  Pogg.  138.  318.) 

BaS2O6 

.     1  :  2242 

Cd(N03)2 
MgSO4      ' 

.     1  :  3483 
.     1  :  6830 

Cuprous  lead  sulphide,  9Cu2S,  2PbS. 

Ba(N03)2 

.     1  :  2677 

3Cu2S,  2PbS. 

BaCl2   . 

.     1  :  3921 

2Cu2S,  2PbS.    Min.  Cuproplumbite. 

Pb(C103)2 

.     1  :  6988 

CdSO4  . 
MnSO4      si- 

.     1  :  3442 
.     I  :  5518 

Copper  phosphorus  sulphide. 
See  Copper  phosphosulphide. 

Salts  of  trivalent  metals  — 

Ammonia  alum     . 
Chrome  alum     '  . 
A12(S04)3      .     7.Vij 

.     1  :  31,896 
.     1  :  58,889 
.     1  :  90,909 

Cupric  platinum  sulphide. 
See  Sulphoplatinate,  cupric. 

Acids  — 

SUCCITIIC 

1-100 

Cuprous  potassium  sulphide,  4Cu2S,  K2S. 

Oxalic  . 

•        J.    •   AvA/ 

.     1  :  162 

(Ditte,  C.  R.  98.  1429.) 

HC1      . 

1  :  733 

H2S04  . 
Citric   .         .        . 

.     1  :  208 
.     1  :20 

Cuprocupric     potassium     sulphide,     3Cu2S, 
2CuS,  K2S. 

Acetic  . 

.    Not  at  all 

Not  decomp.  by  very  dil.  HCl+Aq,  but 

Tartaric        .        . 

«        « 

easily    by    cone.      HCl+Aq    on    warming. 

(Spring  and  de  Boeck,  Bull 

.  Soc.  (2)  58.  165.) 

(Schneider,  Pogg.  138.  311.) 

Copper  poZ^/sulphide,  Cu2S3. 

Amorphous.  Ppt.  Decomp.  by  boiling 
alcohol.  (Rossing,  Z.  anorg.  1900,  25. 413.) 

Cu4S6.  Amorphous.  Ppt.  can  be  boiled 
with  H2O  without  decomposition.  (Rossing, 
Z.  anorg.  1900,  25.  4,  11.) 

Cu2S6.  Ppt.;  insol.  in  alkali  sulphides; 
decomp.  by  cone.  HN03.  (Bodroux,  C.  R. 
1900,  130.  1398.) 

Could  not  be  obtained.  (Rossing,  Z. 
anorg.  1900,  25.  414.) 

Cu2S,.  Ppt.  Decomp.  by  H2O.  Sol. 
in  alkali  and  barium  po]ysulphides+Aq. 
Decomp.  by  colorless  alkali  sulphides +Aq. 
(Rossing,  Z.  anorg.  1900,  25.  407.) 

Cuprous  iron  (ferric)  sulphide,  Cu2S,  Fe2S3. 

Decomp.  by  cone.  HCl+Aq.  Sol.  in  boiling 
HNO3+Aq  of  1.2  sp.  gr.  (Schneider,  J.  pr. 
(2)  38.  569.) 

Min.  Chalcopyrite.  Insol.  in  HCl+Aq. 
When  heated  in  a  sealed  tube  with  H2S+Aq. 
a  portion  of  it  dissolves  with  difficulty  and 
subsequent  deposition  of  S.  (Senarmont,  A. 
ch.  (3)  32.  168.) 

Cuprocupric  iron  (ferric)  sulphide,  Cu2S,  CuS, 

FeS. 

Min.  Bornite.  Sol.  in  HCl+Aq  with  a 
residue  of  S. 


Copper  potassium  pofysulphide,  KCuS4. 

SI.  sol.  in  cold  H2O.     Decomp.  by  hot 
H2O.     Decomp.    by    cone,    and    dil.    HC1, 
H2SO4  and  HNO8.    SI.  sol.  in  alcohol. 
(Biltz  and  Herms,  B.  1907,  40.  977.) 

2CuS3,  K2S.  Decomp.  by  H2O,  NH4OH, 
or  NH4SH+Aq.  (Priwoznik,  B.  5.  1291.) 

K2Cu8Sio.  Easily  sol.  in  H2O.  1  g.  is  sol. 
in  less  than  5  com.  H2O.  Rapidly  decomp.  by 
dil.  acids,  slowly  by  cone,  acids.  SI.  sol.  in 
alcohol.  (Biltz  and  Herms,  B.  1907,  40.  983.) 

Cupric  rubidium  poZi/sulphide,  RbCuS4. 

As  K  salt.  (Biltz  and  Herms,  B.  1907,  40. 
978.) 

Rb2Cu8Sio.  Easily  sol.  in  H20.  Decomp. 
acids.  SI.  sol.  in  alcohol.  (Biltz  and 
Herms,  B.  1907,  40.  985.) 

Cuprous  silver  sulphide,  Cu2S,  Ag2S. 

Min.  Stromeyerite.  Sol.  in  HNO8+Aq 
with  separation  of  S. 

Cu2S,  3Ag2S.    Min.  Jalpaite.    As  above. 

Cuprous  sodium  sulphide,  Na2S,  Cu2S. 
(Bodlander.  Z.  Elektrochem.  1905, 11. 181.) 
Na2S,  2Cu2S.    (Bodlander,  Z.  Elektrochem. 

L905,  11.  181.) 


312 


CUPROCUPRIC  SODIUM  SULPHIDE 


Cuprocu 
Na 


sodium    sulphide,   Cu2S,   CuS, 


Scarcely  decomp.  by  cold  dil.  HCl-fAq; 
cone.  HCl+Aq  decomp.  easily  on  warming, 
without,  however,  dissolving  all  the  Cu2S. 
Completely  decomp.  by  warm  HNO3+Aq. 
(Schneider,  Pogg.  138.  315.) 

Copper  zinc  sulphide,  CuS,  3ZnS. 

Copper  sulphophosphide. 
See  Copper  phosphosulphide. 

Cupric  telluride,  CuTe. 

Cu2Te«.  Insol.  in  H2O.  (Parkmann,  Sill. 
Am.  J.  (2)  3.  335.) 

Cu2Te.    (Brauner,  M.  1889.  423.) 

Croceocobaltic  bromide. 

Co(NH8)4(N02)2Br. 

Very  si.  sol.  in  cold,  easily  in  hot  H2O. 
(Gibbs,  Proc.  Am.  Acad.  10.  1.) 

chloraurate,  2Co(NH8)4(N02)2Cl,  AuCl3. 

Difficultly  sol.  in  H2O. 

chloride,  Co(NH8)4(NO2)2Cl. 

Very  si.  sol.  in  cold  easily  in  hot  H2O,  but 
more  sol.  than  the  sulphate.  (Gibbs.) 

chloroplatinate,  2Co(NH3)4(NO2)2Cl, 

PtCl4. 

Can  be  recrystallised  without  decomp.  with 
difficulty.  (Gibbs  and  Genth,  Sill.  Am.  J.  (2) 
24.  91.) 

chromate,[  Co(NH,)4(NO2)2]2CrO4. 

SI.  sol.  in  H,O.    (Gibbs.) 

bichromate,  [Co(NH8)4(NO2)2]2Cr2O7 

81.  sol.  in  H20.    (Gibbs.) 

periodide,  Co(NH8)4(NO2)2I,  I2. 

Difficultly  sol.  in  cold  H2O  and  alcohol. 
Decomp.  by  hot  H20.  (Gibbs.) 

nitrate,  Co(NH8)4(N02)2NO8. 

SI.  sol.  in  cold,  easily  sol.  in  hot  H2O  or  dil. 
.acids.  Much  more  sol.  than  the  sulphate. 
<Gibbs.) 

Sol.  in  about  400  pts.  cold  H2O.  (Jorgen- 
sen, Z.  anorg.  6.  163.) 

nitrite  cobaltic  nitrite,  3Co(NH8)4rNO2)2, 

Co(N02)8. 

Somewhat  sol.  in  H2O.  (Jorgensen,  Z. 
anorg.  6.  178.) 

nitrite  examine  cobaltic  nitrite, 

Co(NH8)4(N02)2,(N02)2(NH3)2Co(N02)2. 
Nearly  insol.  in  cold,  very  si.  sol.  in  boiling 
H2O.     (Jorgensen.) 


Croceocobaltic  phosphomolybdate, 

[Co(NH3)4(N02)2]20,  24Mo03,P2Ofi. 
SI.  sol.  in  cold,  easily  in  hot  H2O.    (Gibbs, 
Am.  Ch.  J.  3.  317.) 

sulphate,  [Co(NH3)4(Np2)2]2SO4. 

Very  si.  sol.  in  cold  or  hot  H2O;  more 
easily  in  hot  dil.  H2SO4+Aq. 

Cuprammonium  compounds. 
See  Copper  compounds,  ammonia. 

Cupro^rammonium  te^raiodide. 
See  Cupric  letraiodide  ammonia. 


Cupric  acid. 

Known  only  in  solution. 
62.  445.) 


(Kriiger,  Pogg. 


Calcium  cuprate. 

Decomp.  by  H2O  with  evolution  of  oxygen. 
(Kriiger  and  Crum,  A.  56.  213.) 

Cyanhydric  acid,  HCN. 

Miscible  with  H2O,  alcohol,  and  ether  with 
absorption  of  heat. 

Sp.  gr.  of  HCN+Aq. 


%  HCN 

Sp.  gr. 

%  HCN 

Sp.  gr. 

1.60 

0.9979 

4.0 

0.9940 

1.68 

0.9978 

4.6 

0.9930 

1.77 

0.9975 

5.0 

0.9923 

2.0 

0.9974 

5.3 

0.9914 

2.1 

0.9973 

5.8 

0.9900 

2.3 

0.9970 

6.4 

0.9890 

2.5 

0.9967 

7.3 

0.9870 

2.7 

0.9964 

8.0 

0.9840 

3.0 

0.9958 

9.1 

0.9815 

3.2 

0.9952 

10.6 

0.9768 

3.6 

0.9945 

16.0 

0.9570 

(Ure,  Quar.  J.  Sci.  13.  321.) 

2HCN  mixed  with  3H2O  causes  a  diminu- 
tion of  temp,  of  9.75°.  (Bussy  and  Buignet, 
A.  ch.  (4)  3.  231.) 

Miscible  with  volatile  oils  and  other  organic 
compounds. 

Cyanhydric  iodhydric  acid,  HI,  HCN. 

Easily  sol.  in  H2O  or  alcohol,  with  rapid 
decomp.  SI.  sol.  in  ether.  (Gal,  A.  138.  38.) 

Cyanides. 

The  alkali  cyanides  are  easily  sol.  in  H2O; 
those  of  the  alkali-earths  are  less  sol.,  while 
all  others  are  insol.  with  the  exception  of 
Hg(CN)2.  All  cyanides  are  sol.  in  KCN  +Aq. 

Ammonium  cyanide,  NH4CN. 

Unstable;  easily  sol.  in  H2O  and  alcohol. 


CYANIDE,  BARIUM  NICKEL 


313 


Ammonium  cobaltic  mercuric  cyanide. 
See  Cobalticyanide,  ammonium  mercuric. 

Ammonium    cuprous    cyanide.    NH4CN, 

Cu2(CN)2. 

Ppt.    Decomp.  by  acids. 

+H2O.  Sol.  in  H2O,  less  sol.  in  alcohol. 
Decomp.  by  acids  and  alkalies.  (Treadwell 
and  Girsewald,  Z.  anorg.  1904,  39.  90.) 

2NH4CN,  Cu2(CN)2.  SI.  sol.  in  H2O,  but 
decomp.  by  long  boiling  therewith.  Sol.  in 
HCN-f-Aq.  (Dufau,  A.  88.  278.) 

Ammonium  cuprous  cyanide  ammonia, 
NH4CN,  2Cu2(CN)2,  NH3. 

Easily  decomp.  (Treadwell  and  Girse- 
wald, Z.  anorg.  1904,  39.  90.) 

+2H2O.  Insol.  in  cold,  decomp.  by  boiling 
H2O.  Sol.  in  NH4OH+Aq.  (Fleurent,  C.  R. 
1893,  116.  191.) 

NH4CN,  Cu2(CN)2,  3NH3.  Insol.  in  cold, 
si.  sol.  in  boiling  H2O  without  decomp.  Sol. 
in  NH.OH+Aq.  (Fleurent,  C.  R.  1891,  113. 
1046.) 

NH4CN,  2Cu2(CN)2,  2NH,+2H20.  (Fleu- 
rent,  B.  25.  498R.) 

Ammonium  gold  (aurous)  cyanide  NH4CN, 

AuCN. 

Easily  sol.  in  cold  or  warm  H2O  or  in  al- 
cohol. Insol.  in  ether. 

Ammonium  gold   (auric)  mercuric  cyanide, 
basic,  3NH4CN,  2Au2O,  Hg(CN)2,  HgO. 
(Schmidt,  Ch.  Z.  1896,  20.  633.) 

Ammonium  mercuric  silver  cyanide,  basic, 
NH4CN,  2Ag20,  3AgCN,  4Hg(OH)CN  + 


(Schmidt,  Z.  anorg.  1895,  9.  431.) 

Ammonium   nickel   cyanide,   2NH4CN, 

Ni(CN)2. 
Easily  decomposed. 

Ammonium  tungsten  cyanide. 
See  Tungstocyanide,  ammonium. 

Ammonium  zinc  cyanide,  2NH4CN,  Zn(CN)2. 
Sol.  in  H2O. 

Ammonium  cyanide  mercuric  nitrate  silver 
cyanide  basic,  2Hg(OH)NO3,  3NH4CN, 
4AgCN. 
(Schmidt,  Z.  anorg.  1895,  9.  431.) 

Arsenic  incyanide,  As(CN)8. 

Decomp.  by  H2O.  Not  attacked  by  cold 
cone.  H2SO4.  Decomp.  on  heating.  (Guenez, 
C.  R.  1892,  114.  1188.) 


Barium  cyanide,  Ba(CN)2. 

Rather  si.  sol.  in  H2O,  more  easily  in  KCN 
+Aq.  (Schulz,  J.  pr.  68.  257.) 

10  pts.  H2O  dissolve  8  pts.,  and  10  pts.  70% 
alcohol  dissolve  1.8  pts.  Ba(CN)2  at  14.° 
(Joannis,  A.  ch.  (5)  26.  489.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

+2H2O.     Very  deliquescent. 

Ba(CN)2,  BaO.  (Drechsel,  J.  pr.  (2)  21. 
84.) 

Barium    cadmium    cyanide,    Ba(CN)2, 

Cd(CN)2+H20. 

Easily  sol.  in  H2O  and  in  NF4OH+Aq. 
SI.  sol.  in  alcohol.    (Loebe,  Dissert,  1902.) 
2Ba(CN)2,    3CdfCN)2-flOH2O.      Sol.    in 

H2O.    (Weselsky,  B.  2.  590.) 

Barium  cobaltous  cobaltic  cyanide. 
See  Cobaltocobalticyanide,  barium. 

Barium  cuprous  cyanide,  Ba(CN)2,  Cu2(CN)2. 

Sol.  in  H2O  without  decomp.  (Traube,  Z. 
anorg.  1894,  8.  21.) 

+H2O.    (Weselsky,  B.  2. 590.) 

Could  not  be  obtained.  (Grossmann,  Z. 
anorg.  1905,  43.  101.) 

+4H2O.  Decomp.  by  H2O.  (Grossmann, 
Z.  anorg.  1905,  43.  101.) 

2Ba(CN)2,  Cu2(CN)2+6H2O.  Decomp. 
by  H2O.  (Grossmann,  Z.  anorg.  1905,  43. 
105.) 

Barium    gold    (aurous)    cyanide,    Ba(CN)2, 

2AuCN+2H2O. 

SI.  sol.  in  cold  but  easily  sol.  in  hot  H2O. 
SI.  sol.  in  alcohol.  (Lindbom,  Lund  Univ. 
Arsk.  12.  No.6.)  . 

Barium  iridium  cyanide. 
See   Iridicyanide,   barium. 

Barium    manganous    cyanide,    Ba(CN)2, 
2Mn(CN)2. 

Ppt.     (Descamps.) 

See  also  Manganocyanide  and  .Mangani- 
cyanide,  barium. 

Barium    mercuric    cyanide.    (Ba(CN)2, 

Hg(CN)2+3H20. 

Very  hygroscopic.  Very  sol.  in  H2O. 
(Grossmann,  B.  1904,  37.  4142.) 

Barium  mercuric  cyanide  iodide,  Ba(CN)2, 

HgI2+6H20. 
(Varet,  C.  R.  1895,  121.  499.)  . 

Barium    palladium    cyanide,    Ba(CN)2, 

Pd(CN)2+4H20. 
See  Palladocyanide,  barium. 

Barium  nickel  cyanide,  Ba(CN)2,  Ni(CN)2-f- 

3H2O. 

Sol.  in  H20:  decomp.  by  acids  with  pptn 
of  Ni(CN),.  (Weselsky,  B.  2.  590.) 


314 


CYANIDE,  BARIUM  SILVER 


Barium  silver  cyanide,  BaCN)2,  2AgCN  + 

H2O. 
Sol.  in  H2O.    (Weselsky,  B.  2.  589.) 

Barium  zinc  cyanide,  Ba(CN)2,  Zn(CN)2-f 

2H2O. 
Sol.  in  H2O. 

Cadmium  cyanide,  basic,  CdO2H2,  2Cd(CN> 

+4H20. 

SI.  sol.  in  H2O;  insol.  in  alcohol.  (Loebe 
Dissert,  1902,) 

Cadmium  cyanide,  Cd(CN)2. 

SI.  sol.  in  H2O.  100  pts.  H2O  dissolve  1.7 
pts.  Cd(CN)2  at  15°.  (Joannis.) 

Easily  sol.  in  acids;  sol.  in  KCN+Aq. 
Sol.  in  warm  NH4OH+Aq,  but  insol.  in 
(NH4)2CO3+Aq.  (Wittstein.) 

Insol.  in  benzonitrile.  (Naumann,  B 
1914,  47.  1370.) 

Cadmium    calcium    cyanide,    Cd(CN)2, 

4Ca(CN)2+20H2O. 

Sol.  in  H2O  and  in  alcohol.  (Loebe,  Dis- 
sert, 1902.) 

Cadmium  chromic  cyanide. 
See  Chromicyanide,  cadmium. 

Cadmium  cobaltic  cyanide. 
See  Cobalticyanide,  cadmium. 

Cadmium    cuprous    cyanide,    2Cd(CN)2, 

Cu2(CN)2. 

Permanent.  Insol.  in  H2O.  SI.  sol.  in 
cold,  easily  in  warm  HCl+Aq  without  de- 
comp.,  except  by  long  boiling.  Insol.  in 
NH4OH,  or  NH4  salts+Aq.  (Schiiler.) 

Cadmium  cupric  cyanide,  Cd(CN)2,  Cu(CN)2. 
Very  unstable. 

Cadmium  gold  (aurous)  cyanide,  Cd(CN)2, 

2AuCN. 

Nearly  insol.  in  cold  H2O.  SI.  sol.  in  boil- 
ing H2O.  Insol.  in  alcohol.  (Lindbom.)  • 

Cadmium   mercuric    cyanide,    2Cd(CN)2, 

3Hg(CN)2. 

Permanent.  Readily  sol.  in  cold  H2O. 
(Schiiler.) 

Cadmium  mercuric  cyanide  mercuric  iodide, 

Cd(CN)2,    Hg(CN)2,    HgI2+8H20. 

Very  sol.  in  H2O.     (Varet,  Bull.  Soc.  (3) 
6.8.) 

+7H2O.  Sol.  mH2OandinNH4OH+Aq. 
(Varet,  C.  R.  1890,  111,  679.) 

Cadmium  mercuric  cyanide  mercuric  iodide, 

Cd(CN)2,    Hg(CN)2,    HgI2+8H20. 
Very  sol.  in  H2O.     (Varet,  Bull.  Soc.  (3) 
6.  8.)  " 


-f7H2O.    Sol.  inH2OandinNH4OH+Aq. 
(Varet,  C.  R.  1890,  111.  679.) 

Cadmium  mercuric  cyanide  mercuric  iodide 
ammonia,    Cd(CN)2,    Hg(CN)2,    Hgl», 
4NH8. 
Very  easily  decomp.    (Varet,  Bull.  Soc.  (3) 

6.  22.) 

Cadmium  molybdenum  cyanide. 
See  Molybdocyanide,  cadmium. 

Cadmium   potassium    cyanide,    Cd(CN)2, 

2KCN. 

Sol.  in  3  pts.  cold,  and  1  pt.  boiling  H2O. 
Insol.  in  absolute  alcohol.  (Rammelsberg.) 

Cadmium    sodium    cyanide,    Na2Cd2(CN)6 

+3H2O. 

Sol.  in  H20  and  in  alcohol.  (Loebe,  Dis- 
sert, 1902.) 

Cadmium    strontium    cyanide,    Cd(CN)2, 

2Sr(CN)2+3H20. 

Sol.  in  H2O  and  in  alcohol.  (Loebe.  Dis- 
sert. 1902.) 

Cadmium  tungsten  cyanide,  Cd2W(CN)8+ 
8H2O. 

Nearly  insol.  in  H2O. 

SI.  sol.  in  dil.  HC1.  Sol.  in  cone.  NH4OH  + 
Aq. 

Insol.  in  organic  solvents.  (Olsson,  Z. 
anorg.  1914,  88.  68.) 

Cadmium    cyanide    c&hydrazine,    Cd(CN)2, 

(N2H4)2. 

Easily  sol.  in  dil.  acids.  (Franzen.  Z. 
anorg.  1911,  70.  152.) 

Caesium  cuprous  cyanide,   CsCN,  CuCN  + 


H20  separates  CuCN.  (Grossmann,  Z. 
anorg.  1905,  43.  98.) 

2CsCN,  CuCN+H2O.  Sol.  in  H2O. 
(Grossmann,  Z.  anorg.  1905,  43.  98.) 

2CsCN,  SCuCN.  Insol.  in,  and  not  de- 
comp. by  H2O.  (Grossmann,  Z.  anorg.  1905, 
43.  98.) 

Caesium  tungsten  cyanide. 
See  Tungstocyanide,  caesium. 

lalcium  cyanide,  Ca(CN)2. 

Sol.  in  H2O,  but  the  solution  is  very  un- 
stable. (Schulz.) 

Ca(CN)2,  3CaO+15H2O.  Decomp.  by 
H2O.  (Joannis,  A.  ch.  (5)  26.  496.) 

Jalcium  cuprous  cyanide,  Ca(CN)2,  CuCN  + 
4H2O. 

Easily  decomp.  by  H2O.  (Grossmann, 
Z.  anorg.  1905,  43.  106.) 

Ca(CN)2,    3CuCN+8H2O.      Immediately 


CYANIDE  AMMONIA,  CUPRIC  MOLYBDENUM 


315 


decomp.   by  H2O.      (Grossmann,   Z.   anorg. 
1905,  43.  99.) 

Calcium   gold    (aurous)    cyanide,   Ca(CN)2, 

2AuCN+3H2O. 

Easily  sol.  in  hot  or  cold  H2O  or  in  alcohol. 
(Lindbom.) 

Calcium    manganous    cyanide,    Ca(CN)2, 

2Mn(CN)2. 
Ppt.     (Descamps.) 
See  also  Manganocyanide,  calcium. 

Calcium    mercuric    cyanide,    Ca(CN)2, 
2Hg(CN)2+8H20. 

Very  deliquescent.     (Grossmann,  B.  1904, 
37.  4143.) 

2Ca(CN)2,   3Hg(CN)2+6H2O.     Very  sol. 
in  H2O.     (Grossmann,  B.  1904,  37.  4143.) 

Calcium  mercuric  cyanide  iodide,  Ca(CN)2, 

HgI2,  Hg(CN)2+7H20. 
(Varet,  C.  R.  1895,  121.  499.) 

Calcium  nickel  cyanide,  Ca(CN)2,  Ni(CN)2  + 

zH2O. 
Sol.  in  H2O. 

Calcium.  tungsten  cyanide. 
See  Tungstocyanide,  calcium. 

Calcium  zinc  cyanide,  (Ca(CN)2,  Zn(CN)2+ 


Sol.  in  H20  and  in  alcohol.  (Loebe,  Dis- 
sert. 1902.) 

Cerous  cyanide  (?). 

Ppt.  Very  easily  decomp.  (Behringer,  A, 
42.  139.) 

Chromic  cyanide,  with  MCN. 
See  Chromicyanide,  M. 

Chromous  potassium  cyanide. 
See   Chromocyanide,   potassium. 

Cobaltous  cyanide,  Co(CN)2+H2O. 

Insol.  in  H2O.  Easily  sol.  in  NH4OH+Aq 
and  KCN+Aq;  also  in  (NH4)2C03,  or  NH 
succinate+Aq;  insol.  in  NH4NO3,  or  NH4C 
+Aq.  (Wittstein.) 

Cobaltous  cyanide  with  4MCN. 
See  Cobaltocyanide,  M. 

Cobaltic  cyanide  with  3MCN. 
See  Cobaltocyanide,  M. 

Cobalt    gold    (aurous)    cyanide,    Co(CN)2 

2AuCN. 
Insol.  in  H2O  or  cold  HCl+Aq. 


Cobalt  hydrazine  cyanide,  (N2H4)4Co(CN)6. 
Deliquescent.     (Franzen,  Z.  anorg.   1911, 
70.  155.) 

Cobaltous    cyanide    ammonia,    Co(CN)2, 
2NH3.    ' 

Unstable.    (Peters,  B.  1908,  41.  3178.) 

Cuprous  cyanide,  Cu2(CN)2. 

Insol.  in  H2O  and  dil.  acids.  Sol.  in 
NH4OH,  (NH4)2SO4,  or  NH4  succinate-f 
Aq,  and  in  hot  NH4C1,  or  NH4NO3+Aq. 
Sol.  hi  cone.  HCl+Aq.  Sol.  in  KCN+Aq. 

Easily  sol.  in  cone.  NH4SCN  or  KSCN  +  Aq 

SI.  sol.  in  NaSCN+Aq,  (Grossmann,  Z. 
anorg.  1903,  37.  408.) 

SI.  sol.  in  liquid  NH2.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Very  si.  sol.  hi  pyridine.  (Schroeder, 
Dissert.  1902.) 

Mol.  weight  determined  hi  pyridine. 
Werner,  Z.  anorg.  1897,  15.  20.) 

Cupric  cyanide,  Cu(CN)2. 
Easily  decomp.    Insol.  in  H2O. 
Sol.  in  pyridine.    (Schroeder,  Dissert.  1901.) 
Insol.  in  methyl  acetate.     (Naumann,  B. 

1909,  42.  3790.) 

Cuprocupric  cyanide,  Cu(CN)2,  Cu2(CN)2  + 
5H2O. 

Insol.  in  H2O,  but  decomp.  by  boiling.  Sol. 
in  cold  cone.  HCl+Aq.  Sol.  in  NH4OH+Aq. 
(NH4)2CO3+Aq,  and  in  hot  NH4  salts +Aq. 
Easily  sol.  in  KCN+Aq. 

+H2O.    Ppt.    (Dufau.) 

+Cu(CN)2,  2Cu2(CN)2+H20.     Ppt. 

Cuprous    hydrazine    cyanide,    Cu2(CN)2, 

N2HSCN. 

Insol.  hi  alcohol  and  H2O.  (Ferratini, 
C.C.  1912, 1. 1281.) 

Cupric  iridium  cyanide. 
See  Iridicyanide,  cupric. 

Cuprous  lithium  cyanide,  Cu2(CN)2,  LiCN  + 

H20. 

Gradually  decomp.  by  H2O.  (Grossmann, 
Z.  anorg.  1905,  43.  97.) 

Cuprous    magnesium    cyanide,    Cu2(CN)2, 

Mg(CN)2  +  llH20. 

Decomp.  by  H2O.  (Grossmann,  Z.  anorg. 
1905,  43.  103.) 

Cuprous  mercuric  cyanide  bromide,  Cu(CN)2, 

2Hg(CN)2l  HgBr2. 
Sol.  in  H8O.    (Varet,  C.  R.  1890,  110.  148.) 

Cupric  molybdenum  cyanide  ammonia. 
See  Molybdocyanide  ammonia,  cupric. 


316 


CYANIDE,  CUPROUS  POTASSIUM 


Cuprous   potassium   cyanide,   Cu»(CN)2, 
2KCN. 

SI.  sol.  in  H2O,  with  partial  decomp.  De- 
comp.  by  acids,  but  not  by  alkalies. 

Decomp.  by  boiling  H2O.  Sol.  in  NH4OH 
+Aq.  (Fleurent,  C.  R.  1893,  116.  191.) 

Sol.  without  decomp.  in  cone.  KSCN. 
(Grossmann,  Z.  anorg.  1903,  37.  407.) 

Sol.  without  decomp.  in  KCN+Aq. 
(Tread well  and  Girsewald,  Z.  anorg.  1904, 

38.  94.) 

Cu2(CN)2,  KCN+HoO.  Almost  insol.  in 
cold  H2O.  100  cc.  H2O  dissolve  0.0594  g.  at 
15°.  Decomp.  by  much  hot  H2O  with  sep- 
aration of  Ciio(CN)2.  Sol.  in  KCN+Aq  or  in 
NH4OH+Aq.  (Treadwell  and  Girsewald, 
Z.  anorg.  1904,  38.  93.) 

3Cu2(CN)2,  4KCN.    Sol.  in  H2O. 

Cu2(CN)2,  6KCN.    Sol.  in  H2O. 

Cuprous  potassium  cyanide  ammonia. 

Cu2(CN)2,  KCN,  NH3. 
(Treadwell  and  Girsewald,  Z.  anorg.  1904, 

39.  88.) 

Cuprous  potassium  cyanide  potassium  sul- 
phocyanide,  Cu2(CN)2,  4KCN,  2KSCN, 
H2O. 
Easily  sol.  in  cold  H2O.     (Itzig,  B.  1902, 

36.  108.) 

Cupric  potassium  cyanide,  Cu(CN)2,  2KCN. 

Sol.  in  3/4  pt.  H2O  at  15°  and  Vs  pt.  at 
100°.  (Buignet,  J.  Pharm.  1859,  (3),  35.  168.) 

Cuprocupric  potassium  cyanide.   Cu2(CN)2, 

Cu(CN)2,  2KCN. 
(Straus,  Z.  anorg.  1895,  9.  15.) 

Cuprous    rubidium    cyanide,     Cu2(CN)2, 
2RbCN. 

SI.  sol.  in  H20.  Pure  H20  separates  CuCN. 
(Grossmann,  Z.  anorg.  1905,  43.  100.) 

3Cu2(CN)2,  4RbCN.  SI.  sol.  in  H2O. 
Pure  H20  separates  CuCN.  (Grossmann, 
Z.  anorg.  1905,  43.  98.) 

Cuprous  silver  cyanide,  Cu2(CN)2,  2AgCN. 

Ppt. 

Cu2(CN)2,  6AgCN.     Sol.  in  excess  of 
Cu2(CN)2,  KCN+Aq.     (Rammelsberg.) 

Cuprous  sodium  cyanide,  Cu2(CN)2,  2NaCN. 

CTraube,  Z.  anorg.  1894,  8.  21.) 

+4H2O.  Docomp.  by  H2O.  Sol.  in  excess 
of  NaCN+Aq.  (Grossmann,  Z.  anorg.  1905, 
43.  96.) 

Cu2(CN)2,  NaCN+2H2O.  Decomp.  by 
H2Q.  ( Grossmann,  Z.  anorg.  1905,  43.  96.) 

Cu2(CN)2,  4NaCN+6H2O.  Very  sol.  in 
H2O  without  decomp.  (Grossmann/Z.  anorg. 
1905,  43.  96.) 

Cu2(CN)2,  6NaCN+6H2O.     Very  sol.  in 


H2O     without     decomp.       (Grossmann,     Z. 
anorg.  1905,  43.  96.) 

Cuprous    strontium    cyanide,    Cu2(CN)2, 

Sr(CN)2+8H2O, 

H2O  separates  Cu2(CN)2.  (Grossmann,  Z. 
anorg.  1905,  43.  103.) 

Cuprous    cyanide    ammonia,     Cu2(CN)2, 

2NH3. 

Nearly  insol.  in  cold  H2O.  Easily  sol.  in 
NH4OH+Aq  in  absence  of  oxygen.  Insol. 
in  alcohol  and  ether.  Decomp.  by  hot  H2O 
and  acids.  (Treadwell  and  Girsewald,  Z. 
anorg.  1904,  39.  87.) 

Cuprocupric    cyanide    ammonia,    Cu2(CN)2, 
Cu(CN)2,  2NH3. 

(Malmberg,  Arch.  Pharm.  1898,  236.  256.) 

+H2O.  SI.  sol.  in  cold,  decomp.  by  boiling 
H2O.  Sol.  in  NH4OH+Aq.  (Dufau/A.  88. 
278.) 

Cu(CN)2,  Cu2(CN)2  3NH3.  (Mills,  Z. 
Ch.  1867.  545.) 

SI.  decomp.  by  boiling  H20.  Sol.  in 
NH4OH+Aq  and  can  be  recryst.  therefrom. 
Insol.  in  alcohol  and  ether.  Decomp.  by 
alkalies  and  acids.  (Treadwell  and  Girse- 
wald, Z.  anorg.  1904,  39.  96.) 

Cu(CN)2,  Cu2(CN)2,  4NH3.  Insol.  in  cold, 
decomp.  by  hot  H2O.  Sol.  in  NH4OH,  or 
(NH4)2CO3+Aq.  (Treadwell  and  Girse- 
wald, Z.  anorg.  1904,  39.  92.) 

2Cu2(CN)2,  Cu(CN)2,  2NF3.  Insol.  in 
H2O,  alcohol  and  ether.  Sol.  in  NH4OH  + 
Aq.  Decomp.  by  boiling  acids  and  alkalies. 
(Treadwell  and  Girsewald,  Z.  anorg.  1904,  39. 
92.) 

+H2O.    (Monthier,  J.  Pharm.  11.  257.) 

Cu(CN)2,  2Cu2(CN)2,  4NH3.  (Hillen- 
kamp,  A.  97.  218.) 

Cu(CN)2,  2Cu2(CN)2,  6NH3.  (Schiff  and 
Becchi,  A.  134.  33.) 

2Cu(CN)2,     Cu2(CN)2,     2NH3+3H2O. 
(Fleurent,  C.  R,  114.  1060.) 

2Cu(CN)2,  Cu2(CN)2,  4NH3+H2O.  Cor- 
rect formula  for  Cu(CN)2,  Cu2(CN)2,  4NH8. 
(Bouveault,  Bull.  Soc.  (3)4.  641.) 

Cuprous  cyanide  ammonium  sulphocyanide, 

Cu2(CN)2,  3NH4SCN. 
Decomp.  by  H2O.    (Grossmann,  Z.  anore. 
1903,  37.  409. 

Cupric  cyanide  hydrazine,  Cu(CN)2(N2H4). 

Insol.  in  H2O  and  cold  dil.  acids. 

Sol.  in  warm  dil.  acids.  (Franzen,  Z. 
anorg.  1911,70.  154.) 

Cuprous  cyanide  mercuric  iodide,  Cu2(CN)2, 
HgI2. 

Sol.   in  H2O.      (Varet,    Bull.   Soc.    (3)   4. 

484.) 


CYANIDE,  MANGANOUS  STRONTIUM 


317 


Cuprous  cyanide  potassium  sulphocyanide, 

Cu2(CN)2,  3KSCN. 

Decomp.  by  H2O.  (Grossmann,  Z.  anorg. 
1903,  37.  409.) 

Gold  (aurous)  cyanide,  AuCN. 

Insol.  in  H2O,  alcohol,  or  ether.  Not  at- 
tacked by  dil.,  or  cone,  acids,  even  boiling 
aqua  regia. 

Sol.  in  NH4OH+Aq,  also  in  soluble  cy- 
anides +Aq. 

Slowly  decomp.  by  boiling  KOH+Aq,  also 
by  (NH4)2S+Aq. 

Sol.  in  K4Fe(CN)6+Aq.  (Bentel,  Z. 
anorg.  1912,  78.  152.) 

Gold  (auric)  cyanide  with  MCN. 
See  Auricyanide,  M. 

Gold    (auroauric)    mercuric    cyanide    auric 
mercuric    chloride,    4AuCN,    Au(CN)3, 
5Hg(CN)2,  7AuCl3,  5HgCl2. 
(Schmidt,  Ch.  Z.  1896,  20.  633.) 

Gold   (aurous)    potassium   cyanide,   AuCN, 
KCN. 

Sol.  in  7  pts.  cold,  and  less  than  0.5  pt.  boil- 
ing H2O.    SI.  sol.  in  cold,  and  somewhat  more 
sol.  in  boiling  alcohol.     Insol.  in  ether. 
(Himly,  A.  42.  160.) 

Decomp.  by  warm  acids,  even  tartaric,  and 
acetic  acids. 

Gold  (aurous)  sodium  cyanide,  AuCN,  NaCN. 
SI.  sol.  in  cold,  more  easily  in  hot  H20. 
SI.  sol.  in  alcohol.    (Lindbom.) 

Gold   (aurous)   strontium  cyanide,  2AuCN, 

Sr(CN)2+3H20. 
As  the  Na  salt. 

Gold  (aurous)  zinc  cyanide,  2AuCN,  Zn(CN)2. 
Nearly  insol.  in  hot  or  cold  H2O. 
Insol.  in  cold  HCl+Aq. 

Gold  (auric)  cyanide  auric  mercuric  chloride, 

Au(CN)3,  AuCl3,  2HgCl2. 
(Schmidt,  Ch.  Z.  1896,  20.  633.) 

Gold   (auroauric)   cyanide   aurous   mercuric 
chloride,    12AuCN,    3Au(CN)3,   4AuCl, 
2HgCl2. 
(Schmidt,  Ch.  Z.  1896,  20.  633.) 

Gold  (auroauric)  cyanide  mercuric  chloride. 

ISAuCN,  2Au(CN)3,  5HgCl2. 
(Schmidt,  Ch.  Z.  1896,  20.  633.) 

Iridium  cyanide,  Ir(CN)3. 

Insol.  in  H2O.    Sol.  in  HCN  +Aq. 

Iridium  cyanide  with  MCN. 
See  Iridicyanide,  M 


Lanthanum  cyanide,  La(CN)3, 

Ppt.  (Frerichs  and  Smith,  B.  11.  910, 
1151.) 

Lead  cyanide,  Pb(CN)2. 

SI.  sol.  in  cold,  more  in  hot  H2O.  Sol.  in 
HNOs+Aq,  and  KCN+Aq.  Partially  sol.  in 
NH4OH+Aq,  and  NH4  salts+Aq.  Not 
pptd.  in  presence  of  Na  citrate. 

Above  compound  is  2PbO,  Pb(CN)2  + 
H2O.  (Joannis,  A.  ch.  (5)  26.  204.) 

2PbO,  Pb(CN)2+H26.     Insol.  in  H2O. 

Lead  tungsten  cyanide. 
See  Tungstocyanide,  lead. 

Lead  zinc  cyanide,  Pb(CN)2,  2Zn(CN)2. 
Ppt.    (Rammelsberg.) 

Lead  cyanide  chloride,  2Pb(CN)2,  PbCl2. 

Insol.  in  H2O.  (Grissom  and  Thorp,  Am. 
Ch.  J.  10.  229.) 

Lithium  mercuric  cyanide  mercuric  iodide, 

2Li(CN)2,  Hg(CN)2,  HgI2+7H20. 
Deliquescent;  s.ol.  in  H2O.     (Varet,  C.  R. 
111.  526.) 

Magnesium  cyanide,  Mg(CN)2. 

Known  only  in  aqueous  solution  which  de- 
composes on  evaporation.  (Schulz.) 

Magnesium   mercuric   cyanide,   2Mg(CN)2, 

3Hg(CN)2+5H20. 
(Grossmann,  B.  1904,  37.  4143.) 

Magnesium     mercuric     cyanide     mercuric 
bromide,  Mg(CN)2,  Hg(CN)2,  HgBr2  + 
8H2O. 
Very  sol.  in  H2O.     (Varet,  Bull.  Soc.  (3) 

7.  170.) 

Magnesium    mercuric    cyanide    mercuric 
iodide,    Mg(CN)2,    Hg(CN)2,    Hgl  + 
8H2O. 
Sol.  in  H2O.    (Varet,  Bull.  Soc.  (3)  7.  170.) 

Magnesium  platinum  cyanide. 
See  Platinocyanide,  magnesium. 

Magnesium  tungsten  cyanide. 
See  Tungstocyanide,  magnesium. 

Manganous  and  manganic  cyanides. 

See  Manganocyanhydric,  and  Mangani- 
cyanhydric  acids. 

Manganous  strontium  cyanide,  2Mn(CN)2. 

Sr(CN)2. 

Ppt.     (Descamps.) 
See  also  Manganocyanide,  strontium. 


318 


CYANIDE,  MANGANOUS  TUNGSTEN 


Manganous  tungsten  cyanide. 
See  Tungstocyanide,  manganous. 

Manganic  cyanide,  with  MCN. 
See  Manganicyanide,  M. 

Manganous  cyanide  with  MCN. 
See  Manganocyanide,  M. 

Mercuric  cyanide,  basic,  Hg(CN)2,  HgO. 

SI.  sol.  in  cold,  moderately  sol.  in  hot  H2O. 
Sol.  with  decomp.  in  KOH,  KCN,  or  KC1  + 
Aq.  (Johnston.) 

Decomp.  by  H2O  over  80°.  (Holdermann, 
Arch.  Pharm.  1906,  244.  135.) 

Cold  H2O  dissolves  about  1%,  boiling  H2O 
about  5%.  (Borelli,  Gazz.  ch.  it.  1908,  38. 
(1;,  361.) 

1.1%  dissolves  in  H2O  at  ord.  temp. 
(Richard,  J.  Chim.  Phys.  (6)  18.  555.) 

At     0°  1/100  mol.  dissolve  in  1  1.  H2O. 
At  25°    1/32      "  "         "      "        " 

At  90°    1/10      "          "         "      "       " 

(Borelli,  Gazz.  ch.  it.  1908,  38.  (1),  361.) 

1000  cc.  cold  H2O  dissolve  1.35g.  (Holder- 
mann, Arch.  Pharm.  1906,  244.  135.) 

Less  sol.  in  cold  H2O  than  Hg(CN)2. 
(Pieverling,  J.  B.  1899,  783.) 

Somewhat  sol.  in  dil.  alcohol. 

Practically  insol.  in  alcohol,  ether,  C6H6 
and  all  organic  solvents.  (Borelli,  Gazz.  ch. 
it.  1908,  38,  (1),  361.) 

Sol.  in  110  pt.  alcohol  of  90°  Be.  (Richard, 
J.  Chim.  Phys.  (6),  18.  555.) 

3Hg(CN)2,  HgO.  (Joannis,  A.  ch.  (5)  26. 
469.) 

Moderately  sol.  in  H2O.  (Barthe,  J. 
Pharm.  1896,  (6),  3.  186.) 

Very  sol.  in  hot,  less  sol.  in  cold  H2Q. 
(Holdermann,  Arch.  Pharm.  1904,  242.  32!) 

Easily  sol.  in  HC1.  (Joannis,  A.  ch.  1882, 
(5)  26.  511.) 

Hg(CN)2,  3HgO.  More  sol.  in  H2O  than 
Hg(CN)2,  HgO. 

Mercuric  cyanide,  Hg(CN)2. 

Moderately  sol.  in  H2O. 

100  pts.  Hg(CN)2+Aq  sat.  at  101.1°  con- 
tain 35  pts.  Hg(CN)2,  or  100  pts.  H2O  dis- 
solve 53.85  pts.  Hg(CN)2  at  101.1°.  (Grif- 
fiths.) 

Sol.  in  8  pts.  H2O  at  15°.    (Abl.) 

Sol.  in  11  pts.  cold,  and  2.5  pts.  boiling 
H2O.  (Wittstein.) 

8  g.  are  sol.  in  100  g.  H2O  at  -0.45°. 
(Guthrie,  Phil.  Mag.  1878,  (5)  6.  40.) 

100  g.  H2O  dissolve  9.3  g.  at  13.5°.  (Timo- 
feiev,  Dissert.  1894.) 

100  cc.  sat.  solution  contain  9.3  g.  at  20°. 
(Konowalow,  J.  russ.  Soc.  1898,  (4)  30. 
367.) 

Solubility  in  H20  at  25°  =  0.44  mol.  1 
(Sherrill,  Z".  phys.  Ch.  1903,  43.  735.) 


1  1.  H20  dissolves  0.3956  mol.  (Hofmann 
and  Wagner,  Z.  Elektrochem.  1909,  15.  444.) 

100  g.  H2O  dissolve  12.5  g.  at  15°.  (Marsh 
and  Struthers,  Chem.  Soc.  1905,  87.  1879.) 


100  g.  H2O  dissolve  11.27  g.  at  25°.    Sp.  gr. 
solution  =  1.08 13.     (Herz  and  Anders,  Z. 
anorg.  1907,  52.  164.) 

Hg(CN)2+Aq  containing  7.23%  Hg(CN)2 
has  sp.gr.  20°/20°  =  1.0572. 

Hg(CN)2+Aq  containing  9.07%  Hg(CN)2 
hassp.  gr.  20°/20°  =  1.0743. 
(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 19. 
282.) 

Sp.  gr.  at  16°/4°  of  Hg(CN)2+Aq  contain- 
ing 7.8921%  Hg(CN)2  =  1.06376;  containing 
5.4037%  =  1.04246;  containing  7.5009%  = 
1.06049.  (Schonrock,  Z.  phys.  Ch.  1893,  11. 
770.) 

Not  decomp.  by  acids  except  hot  cone. 
H2S04. 

Sol.  without  decomp.  in  HNO3+Aq.  (Ber- 
zelius.) 

1  1.  NH4OH+Aq  (5.2%  NH3)  dissolves 
204.3  g.  at  about  25°.  (Konowalow.) 

Solubility  in  bases. 

1  1.  H2O  containing  0.3286  mols.  KOH  dis- 
solves 0.5179  mols.  Hg(CN)2. 

1  1.  H20  containing  0.2350  mols.  NaOH 
dissolves  0.4840  mols.  Hg(CN)2. 

1  1.  H2O  containing  0.4775  mols.  NaOH 
dissolves  0.5977  mols.  Hg(CN)2. 

1 1.  H2O  containing  0.9475  mols.  NaOH  dis- 
solves 0.79603  mols.  Hg(CN)2. 

1  1.  H2O  containing  0.970  mols.  LiOH  dis- 
solves 0.6543  mols.  Hg(CN)2. 

1  J.  H2O  containing  0.480  mols.  LiOH  dis- 
solves 0.5500  mols.  Hg(CN)2. 

1  1.  H2O  containing  0.243  mols.  LiOH  dis- 
solves 0.4840  mols.  Hg(CN)2. 
(Hofmann    and    Wagner,    Z.    Elektrochem. 
1909,  15.  444.) 

Solubility  in  KCN+Aq  at  25°. 


Concentration  of  KCN 
Mols.  per  litre 

Solubility  of  Hg(CN)2 
Mols.  per  litre 

0.0493 
0.0985 
0.1970 

0.4855 
0.5350 
0.627. 

(Sherrill,  Z.  phys.  Ch.  1903,  43.  719.) 

Solubility  in  Na2CO3+Aq. 

1  1.  H2O  containing  0.4923  mols.  Na2CO3 
dissolves  0.4956  mols.  Hg(CN)2. 

1  1.  H2O  containing  0.2443  mols.  Na2CO3 
dissolves  0.4464  mols.  Hg(CN)2. 

1  1.  H2O  containing  0.1250  mols.  Na2CO3 
dissolves  0.4147  mols.  Hg(CN)2. 

1  1.  H2O  containing  0.0000  mols.  Na2CO3 
dissolves  0.3952  mols.  Hg(CN)2. 
(Hofmann    and    Wagner,    Z.    Elektrochem, 
1909,  15.  444.) 


CYANIDE,  MERCURIC 


319 


Solubility  in  KNO3+Aq  at  25°. 
1  1.  H2O  containing  0.9574  mols.  KNO3 
•dissolves  0.5383  mols.  Hg(CN)2. 
1  1.  H2O  containing  0.4614  mols.  KN03 
dissolves  0.4619  mols.  Hg(CN)2. 
1  1.  H2O  containing  0.0000  mols.  KNO3  dis- 
solves 0.3956  mols.  Hg(CN)2. 
(Hofmann  and  Wagner,  Z.  Elektrochem.  1909 
15.  444.) 

Insol.  in  liquid  CO2.     (Buchner,  Z.  phys 
Ch.  1906,  54.  674.) 
Very  easily  sol.  in  liquid  NH3.    (Franklin 
Am.  Ch.  J.  1898,  20.  829.) 

Solubility  of  Hg(CN)2  in  ethyl  alcohol  at  t° 

Solubility  of  Hg(CN)2  in  ethyl  alcohol  +Aq 
at  25°. 

P  =  g.  alcohol  in  100  g.  alcohol  +Aq. 
Hg(CN)2  =  millimols  Hg(CN)2  in  10  cc.  of 
the  solution. 

p 

Hg(CN)2 

Sp.  gr. 

0 
20.18 
40.69 
70.01 
100 

4.34 
3.47 
3.58 
3.80 
3.25 

1.0813 
1.0339 
1.0006 
0.9419 
0.8552 

(Herz  and  Anders,   .  c.) 

Solubility  of  Hg(CN)2  in  mixtures  of  methyl 
and  ethyl  alcohol  at  25°. 

P  =  %  methyl  alcohol  in  the  solvent. 
Hg(CN)2=g.  Hg(CN)2  in  10  ccm.  of  the 
solution. 
S  25°/4°=Sp.  gr.  of  the  sat.  solution. 

t° 

%  HgCl2 

0 
10 
20 
30 
40 

8.3 
8.8 
9.25 
9.8 
10.3 

(Timofeiev, 

Solubility  of  Hg(CN) 
HeCCN^  —  ff  Hff( 

Dissert.  1894.) 

2  in  methyl  alcohol  at  t°. 
CN)2  in  100  g.  of  the 
ution. 

p 

Hg(CN)2 

S  25°/4° 

sol 

0 
4.37 
10.4 
41.02 
80.69 
84.77 
91.25 
100 

0.819 
0.902 
1.01 
1.67 

2.82 
2.96 
3.09 
3.43 

0.8552 
0.8618 
0.8707 
0.9267 
1.024 
1.034 
1.052 
1.076 

t° 

Hg(CN)2 

0.0 
14.7 
23.4 
27.4 
31.7 
38.1 
44.5 

26.10 
29.17 
32.01 
31.77 
32.53 
33.29 
34.05 

(Herz  and  Kuhn,  Z.  anorg.  1908,  58.  166.) 

(Dukelski,  Z.  anorg.  1907,  53.  337.) 

100  pts.  methyl  alcohol  dissolve  44.2  pts. 
Hg(CN)2  at  19!5°;  100  pts.  ethyl  alcohol 
dissolve  2.09  pts.  at  19.5°.  (de  Bruyn,  Z. 
phys.  Ch.  1892,  10.  784.) 

Sol.  in  2.5  pts.  methyl  alcohol  at  14°;  in 
20  pts.  ethyl  alcohol  at  15°.  (Marsh,  Chem. 
Soc.  1905,  87.  1878.) 

Solubility  of  Hg(CN)2  in  methyl  alcohol + 
Aq  at  25°. 

P  =  g.  alcohol  in  100  g.  alcohol+Aq. 

Hg(CN)2  =  millimols.  Hg(CN)2  in  10  cc.  of 
the  solution. 


100  g.  propyl  alcohol  dissolve  3.79  g. 
Hg(CN)2  at  13.5°.  (Timofeiev,  Dissert. 
1894.) 


Solubility  in  mixtures  of  propyl  and  methyl 
alcohol  at  25°. 

P  =  %  propyl  alcohol  in  the  solvent. 

G  =  g.  Hg(CN)2  in  10  ccm.  of  the  solution. 

S  =  Sp.  gr.  of  the  sat.  solution. 


P 

Hg(CN)2 

Sp.  gr. 

p 

G 

S  25°/4° 

0 
10.60 
30.77 
37.21 
47.06 
64.00 
78.05 
100 

4.34 
4.37 
4.94 
5.40 
6.49 
8.13 
9.75 
13.60 

1.0813 
1.0642 
1.0484 
1.0430 
1.0426 
1.0441 
1  .  0484 
1.0762 

0 
11.11 
23.8 
65.2 
91.8 
93.97 
96.6 
100 

3.43 
2.952 
2.448 
1.048 
0.504 
0.423 
0.398 
0.344 

1.0760 
1.0327 
0.9891 
0.8800 
0.8376 
0.8335 
0.8322 
0.8283 

(Herz  and  Anders,  Z.  anorg.  1907,  62.  165.) 

(Herz  and  Kuhn,  Z.  anorg.  1908,  60.158.) 

320 


CYANIDE  AMMONIA,  MERCURIC  NICKEL 


Solubility  in  mixtures  of  propyl  and  ethyl 
alcohol  at  25°. 
P  =  %  propyl  alcohol  in  the  solvent. 
G  =  g.  Hg(CN)2  in  10  ccm.  of  the  solution. 
S  =  Sp.  gr.  of  the  sat.  solution. 

100  g.  acetonitrile  dissolve  9.58  g.  Hg(CN)2 
at  18°.     (Naumann  and  Schier,  B.  1914,  47. 
249.) 
Solubility  in  benzonitrile  at  18°  =  1.093  g. 
in  100  g.    (Naumann,  B.  1914,  47.  1370.) 
SI.  sol.  in  ethyl  amine.     (Shinn,  J.  phys. 
Chem.  1907,  11.  538.) 
Very  sol.  in  liquid  methyl  amine.    (Gibbs, 
J.  Am.  Chem.  Soc.  1906,  28.  1419.) 
Sol.  in  paratoluidine.    (Werner,  Z.  anorg. 
1897,  15.  7.) 
Mol.  weight  determined  in  pyridine  and 
benzonitrile.     ''Werner,  Z.  anorg.  1897,  15. 
20  and  32.) 
100  g.  pyridine  dissolve  64.8  g.  Hg(CN)2 
at  18°.    (Schroeder,  Z.  anorg.  1905,  44.  6.) 

Solubility  in  pyridine. 

P 

G 

S  25°/4° 

0 
8.1 
17.85 
56.6 
88.6 
91.2 
95.2 
100 

0.819 
0.790 
0.730 
0.521 
0.387 
0.384 
0.364 
0.344 

0.8552 
0.8549 
0.8527 
'  0.8386 
0.8311 
0.8306 
0.8293 
0.8283 

(Herz  and  Kuhn,  1.  c.) 

Sp.  gr.    at    16°/4°    of   Hg(CN)2+alcohol, 
containing  8.2206  %Hg(CN)2=  0.85273;  con- 
taining 5.8652  %  =  0.8348  +  . 
Sp.  gr.  of  16°/4°  of  Hg(CN)2+  pyridine 
containing     29.6018%     Hg(CN)2  =  1.28155; 
containing  23.2275%  =  1.20198. 
(Schonrock,  Z.  phys.  Ch.  1893,  11.  771.) 

1  1.  ether  dissolves  0.01  mol.  at  25°.    (Sher- 
rill,  Z.  phys.  Ch.  1903,  43.  735.).) 
Easily  sol.  in  acetone.    (Krug  and  M'Elroy, 
J.  Anal.  Ch.  6.  84.) 
100  g.  glycerol  dissolve  27  g.  Hg(CN)2  at 
15.5°.     (Ossendowski,   Pharm.   J.    1907,   79. 
575.) 
Nearly  insol.  in  C6H6.     (Sherrill,  Z.  phys. 
Ch.  1903,  43.  735.) 
Sol.   in  methyl   acetate.      (Naumann,    B. 
1909,  42.  3790.) 
100    g.    boiling    methyl    acetate    dissolve 
3.2  g.    (Steiner,  Dissert,  1906.) 

Solubility  of  Hg(CN)2  in  ethyl  acetate  +Aq 
at  25°. 
P  =  g.  ethyl  acetate  in  100  g.  ethyl  acetate 
+Aq. 
Hg(CN)2=rnillimols  Hg(GN)2  in  10  cc.  of 
the  solution. 

Mols.  per 
100Hg(CN)2 

Temp,  of 
Solidification 

Mols.  per 
100Hg(CN)2 

Temp,  of 
Solidification 

7.1 
8.7 
10.1 
10.4 
11.3 
12.9 
13.8 
15.8 
15.9 
17.3 
18.4 
19.3 
20.6 
22.3 

9 
11 
12.3 
12.2 
13 
13.5 
14.5 
16.5 
20.5 
22.5 
28.5 
32 
38 
42 

22.9 
23.7 
25.3 
26.0 
26.6 
27.5 
27.7 
29.0 
32.0 
33.8 
34.4 
38.3 

45 
46 
53 
54.5 
56.6 
68 
70 
86 
111 
122.5 
125 
141 

(Staronka,   Anz.   Ak.   Wiss.   Krakau,   1910. 
372.) 

Solubility  in  quinoline. 

Mols.  per 
100Hg(CN)2 

Temp    of 
Solidification 

Mols.  per 

100Hg(CN)2 

Temp,  of 
Solidification 

4.2 
6.0 
8.2 
9.2 

45° 
54 

89(61) 
99(61) 

13.2 
17.4 
22.5 
27.1 

137° 
161 
180 
192 

p 

Hg(CN)2 

Sp.  gr. 

0 
4.39 
96.76 
100 

4.34 
4.295 
1.056 
0.714 

1.0810 
1.0797 
1.9374 
0.09097 

(Staronka,  1.  c.) 
Solubility  in  aniline. 

Mols.  per 
100Hg(CN)2 

Temp,  of 
Solidification 

Mols.  per 

100Hg(CN)2 

Temp,  of 
Solidification 

(Herz  and  Anders,  Z.  anorg.  1907,  52.  165.) 

Insol.   in   ethyl   acetate.      (Naumann,   B. 
1910,  43.  314.) 
Solubility  in  organic  solvents  at  18-20°. 
100  g.  tetrachlormethane  dissolve  0.001  g. 
Hg(CN)2. 
100    g.     bromoform     dissolve    0.005      g. 
Hg(CN)2. 
100   g.    ethyl   bromide   dissolve   0.013    g. 
Hg(CN)2 
100  g.  ethylene  dibromide  dissolve  0.001  g. 
Hg(CN)2. 
(Sulc,  Z.  anorg.  1900,  25.  401.) 

3.7 

4.9 
5.7 

7.7 
9.2 

26°'(?) 
30.  5(?) 
35     (?) 
38.  5(?) 

14.2 
18.2 
19.7 
23.4 

77°  (?) 
83.  5(?) 
84     (?) 
88.  5(?) 

(Staronka,  1.  c.) 

Mercuric  nickel  cyanide  ammonia,  2Hg(CN)2, 
4Ni(CN)2,  5NH3  +  2H2O. 
(Papiermeister,  Dissert.  1898.) 
5Hg(CN)2,    18Ni(CN)2,    8NH3  +  15H2O. 
(Papiermeister,  Dissert.  1898.) 

CYANIDE,  MERCURIC  ZINC  BROMIDE  AMMONIA 


321 


Mercuric    potassium    cyanide,    Hg(CN)2, 
2KCN. 

Sol.  in  4.4  pts.  cold  H2O;  si.  sol.  in  alcohol; 
decomp.  by  acids. 

100  g.  H2O  dissolve  22.7  g.  (Fronmuller, 
B.  1878,  11.  92.) 

Abundantly  sol.  in  liquid  NH3.     (Frank- 
lin, Z.  phys.  Ch.  1909,  69.  295.) 

Mercuric    silver   cyanide,   basic,    Hg(CN)2, 

HgO,  7AgCN. 
Ppt.     (Bloxam,  B.  16.  2669.) 

Mercuric  silver  cyanide  mercuric  sulphate, 
Hg(CN)2,  2AgCN,  HgS04+H20. 

Mercuric  sodium  cyanide,  Hg(CN)2,  NaCN 


Sol.  in  H2O.  (Grossmann,  B.  1904,  37. 
4141.) 

Mercuric  strontium  cyanide, 

Hg(CN)2Sr(CN)2+5H2O. 
Very  hygroscopic.     Sol.  in  H2O.     (Gross- 
mann, B.  1904,  37.  4142.) 

Mercuric  strontium  cyanide  iodide,  Sr(CN)2 

HgI2,  Hg(CN)2+7H20. 
(Varet,  C.  R.  1895,  121.  499.) 

Mercuric  thallium  cyanide,  Hg(CN)2,2TlCN. 
Easily  sol.  in  H2O.    100  pts.  H2O  dissolve 
7.9  pts.  at  1°,  and  10.3  pts.  at  10°.     (Fron- 
muller, B.  11.  92.) 

Mercuric  zinc  cyanide,  4Zn(CN)2,  Hg(CN)2. 
Insol.  in  H2O.     (Dunstan,  Chem.  Soc.  6. 
666.) 

Mercuric    zinc    cyanide    mercuric    bromide 
ammonia,    Hg(CN)2,    Zn(CN)2,   HgBr2, 
4NH3. 
Decomp.  by  H2O.    SI.  sol.  in  cold  NH4OH 

+Aq.    (Varet,  C.  R.  1889,  109.  810.) 

Mercuric  cyanide  ammonia,  Hg(CN)2,  NH3. 

Very  sol.  in  H2O,  NH4OH  +  Aq,  and  alcohol. 
(Varet,  C.  R.  1889,  109.  903.) 

SI.  sol.  in  H2O.  (Schmidt,  B.  1894,  27. 
232.) 

8Hg(CX)2,  2NH3-f-KH20.  Easily  de- 
camp. (Varet,  Bull.  Soc.  (3)  6.  221.) 

Mercuric     cyanide     bromide,     Hg(CN)2, 

HgBr2. 

Very  si.  sol.  even  in  boiling  H20.  (Prussia, 
Gazz.  ch.  it.  1898,  28,  (2),  114.) 

Mercuric  cyanide  barium  bromide,  2Hg(CN)2 

BaBr2+6H2O. 

Easily  sol.  especially  in  hot  H2O  and  al- 
cohol. (Varet,  C.  R.  1895,  121.  398.) 


Mercuric    cyanide    cadmium    bromide, 
Hg(CN)2,  CdBr2+3H2O. 

Sol.  in  H2O  and  NH4OH+Aq.  (Varet, 
Bull.  Soc.  (3)  5.  8.) 

2Hg(CN)2,  CdBr2+4.5  H2O.  Sol.  in  H2O 
and  in  NH4OH+Aq.  (Varet,  C.  R.  1890, 
111.  680.) 

Mercuric  cyanide  cadmium  bromide  ammonia 

2Hg(CN)2,  CdBr2,  4NH3+2H2O. 
Decomp.  by  H2O. 

SI.  sol.  in  NH4OH+Aq.  (Varet,  C.  R. 
1891,  112.  535.) 

Mercuric     cyanide     calcium     bromide, 
2Hg(CN)2,  CaBr2+5H2O. 

Sol.  in  1  pt.  cold,  and  0.25  pt.  boiling  H2O; 
also  in  2  pts.  cold,  and  1  pt.  boiling  90% 
alcohol.  (Custer.) 

+7H20.     (Varet,  C.  R.  1895,  121.  399.) 

Mercuric  cyanide  cupric  bromide  ammonia, 

2Hg(CN)2,  CuBr2,  4NH3. 
Decomp.  by  H2O;  si.  sol.  in  NH4OH+Aq. 
(Varet,  Bull.  Soc.  (3)  6.  221.) 

Mercuric  cyanide  lithium  bromide,  2Hg(CN)2 

2LiBr+7H20. 
Deliquescent.    (Varet,  C.  R.  111.  526.) 

Mercuric  cyanide  magnesium  bromide. 

See  Magnesium  mercuric  cyanide  mercuric 
bromide. 

Hg(CN)2,  2KBr.     Very  sol.  in  H2O. 
(Harth,  Z.  anorg.  1897,  14.  351.) 

Mercuric     cyanide     potassium     bromide, 

Hg(CN)2,  KBr+2H*2O. 
"  Sol.  in  13.34  pts.  H2O  at  18°,  and  less  than 


1  pt.  boiling 


ipts. 
H2O. 


(Brett.) 


Sol.  without  decomp.  in  hot  dil.  H2SO4, 
HNO3,  or  HCl+Aq.  (Brett.) 

Contains  1^H2O.  (Berthelot,  A.  ch.  (5) 
29.  226.) 

Mercuric  cyanide  sodium  bromide,  Hg(CN)2, 


Sol.  in  H2O  and  alcohol. 

Mercuric  cyanide  strontium  bromide, 

2Hg(CN)2,  SrBr2+6H2O. 
Sol.  in  H2O  and  in  alcohol.    (Varet,  C.  R. 
1895,  121.  399.) 

Mercuric    cyanide    zinc    bromide,    HgBr» 

Hg(CN)2,  Zn(CN)2+8H20. 
Sol.  in  H2O  and  NH4OH+Aq.     (Varet, 
Bull.  Soc.  (3)  5.  8.) 

Mercuric   cyanide   zinc   bromide   ammonia, 

HgBr2,  Hg(CN)2,  Zn(CN),,  4NH3. 
As  the  corresponding  chloride.     (Varet.)i 


322 


CYANIDE  CHLORIDE,  MERCURIC 


Mercuric  cyanide  chloride,  Hg(CN)2,  HgCl2. 
Sol.  in  H2O.     Decomp.  by  alcohol,  which 
dissolves  out  HgCl2. 

Mercuric    cyanide    ammonium    chloride, 

Hg(CN)2,  NH4C1. 

Sol.  in  H2O  and  alcohol.     (Poggiale.) 
Hg(CN)2>  4NH4C1. 

Mercuric  cyanide  barium  chloride,  2Hg(CN)2, 

BaCl2+4H2O. 

Efflorescent.   Easily  sol.  in  H2O  and  alcohol 
+6H2O.    (Dexter.) 

Mercuric  cyanide  barium  chloride  ammonia, 

2Hg(CN)2,  BaCl2,  4NH3. 
Decomp.  by  H26.    SI.  sol.  in  NH4OH+Aq. 
«Varet,  Bull.^Soo.  (3)  6.  221.) 

Mercuric    cyanide    cadmium    chloride, 

Hg(CN)2,    CdCl2+2H2O. 
Sol.  in  H2O  and  NH4OH-f  Aq.     (Varet, 
Bull.  Soc.  (3)  6.  8.) 

Mercuric    cyanide    calcium    chloride, 

2Hg(CN)2,  CaCl2+6H20. 
Efflorescent.     Very  sol.  in  H2O.     (Varet, 
C.  R.  1895,  121.  349.) 

Mercuric  cyanide  cerium  chloride,  3Hg(CN)2, 
CeCl3+8H20. 

Very  sol.  in  H2O.  (Ahlen,  Bull.  Soc.  (2) 
27.  365.) 

Mercuric    cyanide    cobaltous    chloride, 

Hg(CN)2,  2CoCl2+4H2O. 
Sol.  inH2O.    (Poggiale.) 
2Hg(CN)2,   CoCl2+7H2O.     (Dexter.) 

Mercuric  cyanide  cupric  chloride,  Hg(CN)2, 
CuCl2-f-6H20. 

Efflorescent. 

Sol.  in  H2O  and  in  NH4OH+Aq.  (Varet. 
C.  R.  1888,  107. 1002.) 

2Hg(CN)2,    CuCl2+6H2O.      Efflorescent. 

Very  sol.  in  H2O  and  in  NH4OH+Aq. 
(Varet,  C.  R.  1888,  107.  1002.) 

Mercuric  cyanide  cupric  chloride  ammonia, 

2Hg(CN)2,  CuCl2,  4NH3. 
Decomp.  by  H2O.    SI.  sol.  in  cold  NH4OH 
+Aq.    (Varet,  Bull.  Soc.  (3)  6.  221.) 

Mercuric   cyanide    didymium   chloride, 

3Hg(CN)2,  DiCl3+8H2O. 
Very  sol.  in  H2O.    (Ahlen.) 

Mercuric  cyanide  erbium  chloride,  3Hg(CN)2, 

ErCl3+8H2O. 
Easily  sol.  in  H20.    (Ahle"n.) 

Mercuric    cyanide   hydrazine    chloride, 

Hg(CN)2,  N2H4,  HC1. 
Very  sol.  in  H2O. 


Nearly  insol.  in  alcohol  and  ether.  (Fer- 
ratini,  Gazz.  ch.  it.  1912,  42.  (1),  154.) 

Mercuric  cyanide  ferric  chloride,  2Hg(CN)2, 
FeCl3+3^H20. 

(Dexter.) 

Mercuric  cyanide  lanthanum  chloride, 

3Hg(CN)2,  LaCl3+8H2O. 
Very  sol.  in  H2O.    (Ahlen.) 

Mercuric  cyanide  magnesium  chloride, 

2Hg(CN)2,  MgCl2+2H2O. 
Easily  sol.  in  H2O  and  dil.  alcohol.    (Pog- 
giale.) 

Mercuric     cyanide     manganous     chloride, 

Hg(CN)2,  MnCl2+3H2O. 
Efflorescent.    Very  sol.  in  H2O.    (Poggiale.) 

Mercuric  cyanide  nickel  chloride,  Hg(CN)2, 

NiCl2+6H20. 

Deliquescent.     Sol.  in  H2O.     (Poggiale.) 
2Hg(CN)2,   NiCl2+7H2O.     (Dexter.) 

Mercuric   cyanide   chloride   nickel   chloride 
oxychloride,  1  !Hg(CN)2, 8HgC]2, 2NiCl2, 
8Ni(OH)Cl+76H2O. 
(Papiermeister,  Dissert.  1898.) 

Mercuric    cyanide    potassium    chloride, 

Hg(CN)2,    KC1+H20. 
Sol.  in  6.75  pts.   H2O   at   18°.      (Brett.) 
Sol.  in  alcohol. 

Mercuric  cyanide  sodium  chloride,  Hg(CN)2, 

NaCl. 

Easily  sol.  especially  in  hot  H2O;  insol.  in 
alcohol.  (Poggiale.) 

Mercuric    cyanide    strontium    chloride, 

2Hg(CN)2,  SrCl2+6H2O. 
Easily  sol.  in  H2O  and  dil.  alcohol.    (Varet, 
C.  R.  1895, 121.  349.) 

Mercuric  cyanide  yttrium  chloride,  3Hg(CN)2 

YC13-|-8H2O. 

Easily  sol.  in  H2O.  (Ahlen,  Bull.  Soc.  (2) 
27.  365.) 

Mercuric  cyanide  zinc  chloride,  2Hg(CN)2, 

ZnCl2+6H20. 

Efflorescent.     Sol.  in  H2O.     (Kane.) 
HgCl2,   Hg(CN)2,   Zn(CN)2+7H2O.     Ef- 

florescent.    Very  sol.  in  H2O.     (Varet.  Bull. 

Soc.  (3)  5.  8.) 

Mercuric  cyanide  zinc  chloride  ammonia, 
HgCl2,  Hg(CN)2,  ZnCl2,  4NH3. 

Decomp.  by  H2O.  Sol.  in  NH4OH-f  Aq. 
(Varet,  Bull.  Soc.  (3)  6.  221.) 

Hg(CN)2,  Zn(CN)2,  HgCl2,  6NH3.  (Varet, 
C.  R.  106.  1080.) 


CYANIDE  ZINC  NITRATE,  MERCURIC 


323 


Mercuric  cyanide  potassium  chromate. 
See  Chromate  mercuric  cyanide,  potassium. 

Mercuric    cyanide    potassium   ferrocyanide, 

3Hg(CN)2,  K4Fe(CN)8+4H2O. 
Readily  sol.  in  H2O. 

Mercuric    cyanide    hydrazine,    Hg(CN)2, 
N2H4. 

Very  sol.  in  H2O  with  partial  decomp. 
(Hofmann  and  Marburg,  A.  1899,  305.  215.) 

Hg(CN)*,  N2H4.  Ppt.  (Franzen,  Z.  anorg. 
1911,  70.  154.) 

Mercuric    cyanide    potassium    hydroxide, 
Hg(CN)2,  KOH. 

(Hofmann  and  Wagner,  B.  1908,  41.  321.) 

+1HH2O.  (Hofmann  and  Wagner,  B. 
1908,  41.  1630.) 

2Hg(CN)2,  KOH-f-H2O.    Very  sol.  in  H2O. 

(Hofmann  and  Wagner,  B.  1908,  41.  320.) 

Mercuric    cyanide    sodium    hydroxide, 

Hg(CN)2.NaOH  +  l^H2O  or  H2O. 
(Hofmann  and  Wagner,  B.  1908,  41.  1631.) 

Mercuric  cyanide  barium  iodide,  2Hg(CN)2, 

BaI2+4H2O. 

Slowly  deliquescent.  Sol.  in  16.5  pts.  cold, 
and  0.4  pt.  boiling  H2O.  Sol.  in  22.5  pts. 
cold,  and  1.6  pts.  hot  90%  alcohol.  Solution 
is  decomp.  on  boiling.  (Custer.) 

Mercuric  cyanide  cadmium  iodide,  Hg(CN)2, 

Cd(CN)2,HgI2+8H20. 
See  Cadmium  mercuric  cyanide  mercuric 
iodide. 

Mercuric  cyanide  caesium  iodide,  Hg(CN)2, 
Csl. 

Recryst.  from  H2O  without  decomp. 

Decomp.  by  acids.  (Mathewson  and 
Wells,  Am.  Ch.  J.  1903,  30.  433.) 

Mercuric  cyanide  calcium  iodide,  2Hg(CN)2, 

CaI2+6H2O. 

SI.  efflorescent.  More  sol.  in  H2O  than 
corresponding  Sr.  comp.  (Custer.) 

Mercuric  cyanide  lithium  iodide,  Hg(CN)2, 

2Li(CN)2,  HgI2+7H2O. 
See   Cyanide,   lithium  mercuric   mercuric 
iodide. 

Mercuric    cyanide    magnesium    iodide, 
Hg(CN)2,   Mg(CN)2,   HgI2+8H2O. 
See  Cyanide,  magnesium  mercuric  mercuric 
iodide. 

Mercuric  cyanide  potassium  iodide.  Hg(CN)2 
KI. 

Sol.  in  16  pts.  cold,  and  less  hot  H2O.  Sol 
in  96  pts.  cold  alcohol  of  34°  Baume.  (Cail- 
lot.)  SI.  sol.  in  ether.  Decomp.  by  acids. 

3Hg(CN)2,  2KI-f-3^H2O.     (Berthelot.) 


Mercuric  cyanide  sodium  iodide,  Hg(CN)2, 
NaI+2H2O. 

Sol.  in  4}/£  pts.  H2O  at  18°,  and  «/7  pt. 
Doiling  H2O. 

Sol.  in  2  pts.  boiling,  and  6^  pts.  cold 
90%  alcohol.  (Custer.) 

Mercuric  cyanide  strontium  iodide, 

2Hg(CN)2,  SrI2+6H2O. 
Sol.  in  7  pts.  H2O  at  18°,  and  1A  pt.  at  b.-pt. 
Sol.  in  4  pts.  90%  alcohol  at  18°,  and  Y2  pt. 
at  b.-pt.     (Custer.) 

Mercuric   cyanide   zinc   iodide,    2Hg(CN)2, 

ZnI2+6H2O. 
Efflorescent;  sol.  in  H2O. 

Mercuric  cyanide  iodide  potassium  cyanide, 

HgI2,  Hg(CN)2,  2KCN. 
Easily    decomp.    by    dil.    acids.      (Rupp. 
Apoth.  Ztg.,  23.  374.) 

Mercuric  cyanide  cadmium  nitrate, 

2Hg(CN)2,  Cd(NO3)2+7H2O. 
Decomp.  by  H2O,  not  by  alcohol.     (Ny- 
lander,  J.  B.  1859  271.) 

Mercuric  cyanide  cobalt  nitrate,  2Hg(CN)2, 

Co(NO3)2  +7H2O. 

Decomp.  by  H2O,  not  by  alcohol.  (Ny- 
lander.) 

Mercuric  cyanide  copper  nitrate,  Hg(CN)2, 

Cu(NO3)2+5H2O. 

Decomp.  by  H2O,  not  by  alcohol.  (Ny- 
lander.) 

Mercuric  cyanide  ferrous  nitrate,  2Hg(CN)2, 

Fe(NO3)2+7H2O. 

Decomp.  by  H^O,  net  by  alcohcl.  (Ny- 
lander.) 

Mercuric  cyanide  manganous  nitrate, 
Hg(CN)3,  Mn(NO3)2+5H,O. 

Decomp.  by  H2O,  not  by  alcohol.  (Ny- 
lander.) 

2Hg(CN)2,  Mn(NO3)2+7H2O.     As  above. 

Mercuric  cyanide  nickel  nitrate,  2Hg(CN)2, 

Ni(NO3)2+7H2O. 

Decomp.  by  H2O,  not  by  alcohol.  (Ny- 
lander.) 

Mercuric  cyanide  silver  nitrate,  2Hg(CN)2, 
AgNO3+2H2O. 

SI.  sol.  in  cold,  more  readily  in  hot  H20. 
Sol.  with  decomp.  in  HNO8+Aq. 

As  sol.  in  alcohol  as  in  H2O. 

Mercuric   cyanide   zinc   nitrate,   2Hg(CN)2, 

Zn(NO3)2+7H2O. 

Sol.  in  H2O  with  decomp.  Not  decomp.  by 
alcohol.  (Nylander,  J.  B.  1859.  271.) 


324 


CYANIDE,  MERCURIC  NITRATE  SILVER  CYANIDE,  BASIC 


Mercuric  cyanide  nitrate  silver  cyanide,  basic, 

Hg(NO3)CN,  lOAgCN,  Hg(OH)NO3. 
(Schmidt,  Z.  anorg.  1895,  9.  431.) 

Mercuric  cyanide  potassium  selenocyanide, 

Hg(CN)2,  KSeCN. 

SI.  sol.  in  cold,  much  more  easily  sol.  in  hot 
H2O  or  alcohol.  Traces  dissove  in  ether. 
(Cameron  and  Davy,  C.  N.  44.  63.) 

Mercuric  cyanide   nickel   sulphate, 

Hg(CN)2,  NiSO4+9H2O. 
(Papiermeister,     Dissert.     1898.) 

Mercuric  cyanide  ammonium  •sulphocyanide, 

Hg(CN)2,  NH4SCN. 

Easily  sol.  in  hot  H2O.  (Cleve,  Bull.  Soc. 
(2)  23.  71.) 

Mercuric    cyanide    barium    sulphocyanide, 

2Hg(CN)2,  Ba(SCN)2-f-4H2O. 
Permanent.    Sol.  in  hot  H2O.    (Cleve.) 

Mercuric   cyanide   cadmium   sulphocyanide, 

2Hg(CN)2,  Cd(SCN)2+4H20. 
Permanent.    Sol.  in  hot  H2O.     (Cleve.) 

Mercuric  cyanide  calcium  sulphocyanide, 

2Hg(CN)2,  Ca(SCN)2+8H2O. 
Sol.  in  H2O.    (Cleve.) 

Mercuric     cyanide     cerium     sulphocyanide, 

3Hg(CN)2,  Ce(SCN)3  +  12H2O. 
Easily  sol.  in  hot  H2O.    (John.) 

Mercuric  cyanide  didymium  sulphocyanide, 

3Hg(CN)2,  Di(SCN)3+6H2O. 
SI.  sol.  in  cold,  easily  in  hot  H2O.    (Cleve.) 

Mercuric    cyanide     erbium    sulphocyanide, 

3Hg(CN)2,  2Er(SCN)3  +  12H2O. 
SI.  sol.  in  cold,  easily  in  hot  H2O.    (Cleve.) 

Mercuric  cyanide  lanthanum  sulphocyanide, 

3Hg(CN)2,  La(SCN)3  +  12H2O. 
Very  sol.  in  H2O.    (Cleve.) 

Mercuric  cyanide  magnesium  sulphocyanide, 

2Hg(CN)2,  Mg(SCN)2+4H20.    ' 
Permanent.    Easily  sol.  in  hot  H2O. 
(Cleve.) 

Mercuric  cyanide  potassium  sulphocyanide, 

.    Hg(CN)2,  KSCN. 

Permanent.  Easily  sol.  in  hot  H2O. 
(Cleve.) 

+2H2O.     (Philip,  Z.  Ch.  1867.  552.) 

Mercuric  cyanide   rubidium   sulphocyanide, 

Hg(CN)2  Rb(SCN). 

Sol.  in  hot  H2O  without  decomp.  (Gross- 
mann,  B.  1904,  37.  1259.) 


Mercuric  cyanide  samarium  sulphocyanide, 

3Hg(CN)2,  Sm(SCN)2  +  12H2O. 
Easily  sol.  in  H2O.    (Cleve.) 

Mercuric    cyanide     sodium    sulphocyanide, 

Hg(CN)2,  NaSCN+2H2O. 
Efflorescent.     Sol.  in  H26.     (Cleve,  Bull. 
Soc.  (2)  23.  71.) 

Mercuric  cyanide  strontium  sulphocyanide, 

2Hg(CN)2,    Sr(SCN)2+4H2O. 
Efflorescent.     (Cleve.) 

Mercuric    cyanide    yttrium    sulphocyanide, 

3Hg(CN)2,  Y(SCN)3  +  12H2O.      . 
SI.  sol.  in  warm,  much  less  in  cold  H2O. 
(Cleve.) 

Mercuric    cyanide    zinc    sulphocyanide, 

2Hg(CN)2,   Zn(SCN)2+4H2O. 
SI.  sol.  in  H2O.    (Cleve.) 

Mercuric   cyanide   zinc    sulphocyanide    am- 
monia, 2Hg(CN)2,  Zn(SCN)2,  3NH3. 
Not  efflorescent.    Decomp.  by  H2O. 

Mercuric    cyanide    potassium    thiosulphate, 

Hg(CN)2,  K2S203.. 
Permanent.    Sol.  in  H2O.    (Kessler.) 
+H2O.    (Fock  and  Klliss,  B.  24.  1355.) 

Molybdenum  hydroxyl  potassium  cyanide, 
K3Mo(OH)2(CN)5. 

(Rosenheim  and  Koss,  Z.  anorg.  1906,  49. 
155.) 

K5Mo(OH)2(CN)8.  Very  sol.  in  H2O. 
(Rosenheim  and  Koss.) 

Molybdenum  cyanide  with  MCN. 
See  Molybdocyanide  M. 

Molybdenyl    potassium    cyanide, 
MoO2(CN)2,  2KCN. 

Very  sol.  in  H2O.  Aqueous  solution  is 
stable  in  presence  of  alkalies. 

Insol.  in  alcohol.  (Pechard,  C.  R.  1894, 
118.  805.) 

Mo02(CN)2,  3KCN.  Sol.  in  H2O.  Insol. 
in  alcohol.  (Hofmann,  Z.  anorg.  1896,  12. 
287.) 

+H2O.  Sol.  in  H2O.  Insol.  in  alcohol. 
(Hofmann.) 

+4H2O.  Sol.  in  H2O.  Insol.  in  alcohol. 
(Hofmann.) 

Nickel  cyanide,  Ni(CN)2+zH2O. 

Insol.  in  H^O.1?  Insoh  in  cone.  HC1,  H2SO4, 
or  HNOs+Aq,  but  decomp.  by  heating  there- 
with. Sol.  in  NH4OH,  warm  (NH4)2SO4, 
or  NH4  succinate+Aq;  also  in  KCN+Aq 
SI.  sol.  in  NH4C1,  or  NH4NO3+Aq.  (Witt- 
stein.) 

Insol.  in  methyl  acetate.     (Naumann    B 
1909,  42.  3790.) 


CYANIDE,  POTASSIUM  VANADIUM 


325 


+3H20, 

and     +5^H2O.       (Papiermeister,     Dissert. 
1898.) 

+4H2O.  (Hofmann  and  Hochtlen,  B. 
1903,  36.  1149.) 

Nickel  potassium  cyanide,  Ni(CN)2,  2KCN 
+H20. 

Sol.  in  H2O.  Decomp.  by  acids  with  residue 
of  insol.  Ni(CN)2. 

+  3^H2O.    (Rammelsberg.) 

Nickel  sodium  cyanide,  Ni(CN)2,  2NaCN  + 

3H20. 

Sol.  in  H20:  decomp.  by  acids  with  residue 
of  Ni(CN)2. 

Nickel  strontium  cyanide,  Ni(CN)2,  Sr(CN)2 

+zH2O. 
Sol.  in  H2O.    (Handl,  J.  B.  1859.  273.) 

Nickel  cyanide  ammonia,  Ni(CN)2,  NH3  + 


Scarcely  attacked  by  H2O  or  dil.  acids. 

Sol.  in  cone.  H2SO4.  Sol.  in  (NH4)2CO3  + 
Aq,  cone.  NH4OH+Aq.  (NH4)2C2O4+Aq, 
(NH4)2S+Aq,  and  KCN+Aq.  Decomp. 
by  boiling  with  NaOH  or  KOH.  (Bernoulli 
and  Grether,  Ch.  Z.  1901,  25.  436.) 

Nickel     cyanide     ^nhydrazine,     Ni(CN)2, 

(N2H4)3. 
Ppt.     (Franzen,  Z.  anorg.  1911,  70.  155.) 

Osmium  cyanide,  Os(CN)2(?). 

Insol.  in  H2O;  not  attacked  by  acids. 
See  also  Osmocyanhydric  acid. 

Osmium  potassium  cyanide. 
See  Osmocyanide,  potassium. 

Palladous  cyanide,  Pd(CN)2. 

Insol.  in  H2O.  Insol.  in  dil.  acids.  Sol. 
in  KCN  or  NH4OH+Aq,  also  in  cone.  HCN 
+Aq. 

Platinous  cyanide,  Pt(CN)2. 

Insol.  in  H2O,  alkalies,  or  acids.  Sol.  in 
KCN+Aq.  When  freshly  pptd.,  sol.  in 
NH4OH+Aq. 

Platinous  cyanide  with  MCN. 
See  Platinocyanide,  M. 

Potassium  cyanide,  KCN. 

Deliquescent.    Very  sol.  in  H2Q. 

100  pts.  KCN+Aq,  sat.  at  b.-pt.  103.3,° 
contain  55  pts.  KCN,  i.  e.  100  pts.  H2O  dis- 
solve 122.2  pts.  KCN  at  103.3.°  (Griffiths.) 

KCN+Aq  containing  3.25%  KCN  has 
sp.  gr.  =  1.0154;  6.5%  KCN,  1.0316.  (Kohl- 
rausch,  W.  Ann.  1879.  1.) 

KCN+Aq  containing  9.64%  KCN  has 
sp.  gr.  20°/20°  =  1.0514. 


KCN+Aq  containing  14.42%  KCN  has 
sp.  gr.  20°/20°  =  1.0768.  (Le  Blanc  and  Roh- 
land,  Z.  phy.  ch.  1896,  19.  278. 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  829.) 

Almost  insol.  in  absolute  alcohol. 

Sol.  in  80  pts.  95%  alcohol  when  boiling, 
and  easily  sol.  in  35%  alcohol.  (Geiger,  A.  1. 
50.) 

100  pts.  absolute  methyl  alcohol  dissolve 
4.91  pts.  at  19.5°;  100  pts.  absolute  ethyl 
alcohol  dissolve  0.87  pt.  at  19.5°.  (de  Bruyn, 
Z.  phys.  Ch.  10.  783.) 

Insol.  in  methyl  acetate  (Naumann, 
B.  1909,  42.  3790) ;  ethyl  acetate.  (Naumann, 
B.  1904,  37.  3601.) 

100  g.  glycerol  dissolve  32  g.  KCN  at  15.5°. 
(Ossendowski,  Pharm.  J.  1907,  79.  575.) 

Sol.  in  CS2  when  pure.  (Loughlin,  J.  B. 
1875.  234.) 

Wholly  insol.  in  CS2.  (Moldenhauer,  Z. 
anal.  16. 199.) 

SI.  sol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1369.) 

Potassium  chromium  Mroxide  pentacyanide, 

K5[(Cr04)2(CN)6]+5H20. 
Very  hygroscopic. 

Sol.  in  H2O.  (Riesenfeld,  B.  1908,  41. 
3548.) 

Potassium  -chromium  tetroxide  cfo'cyanide 
ammonia,  K2[CrO4(CN)2NH3]+5H2O. 

Hygroscopic  in  the  ah1. 

Easily  sol.  in  H2O  and  in  NH4OH+Aq. 
(Riesenfeld,  B.  1908,  41.  3545.) 

Potassium  rhodium  cyanide. 
See  Rhodocyanide,  potassium. 

Potassium  ruthenium  cyanide. 
See  Ruthenocyanide,  potassium. 

Potassium  silver  cyanide,  KCN,  AgCN.    . 
Sol.  in  4.7  pts.  H2O  at  15°,  4  pts.  at  20°, 
and  in  much  less  at  higher  temp.    Sol.  in  25 
pts.  85%  alcohol.    (Baup,  A.  ch.  (3)  53.  464.) 

Potassium   silver   sodium   cyanide,   2KCN, 

NaCN,  3AgCN. 

Sol.  in  4.4  pts.  H2O  at  15°,  and  22  pts.  85% 
alcohol  at  17°.  (Baup.) 

Potassium  tungsten  cyanide. 
See  Tungstocyanide,  potassium. 

Potassium  uranyl  cyanide, 

(UO,)(CN)t,  2KCN. 

Ppt.  Sol.  in  H2O.  SI.  sol.  in  presence  of 
large  excess  of  KCN.  (Aloy,  A.  ch.  1901,  (7) 
24.  417.) 

Potassium  vanadium   cyanide,    K3V(CN)fi. 

Readily  sol.  in  H2O;  decomp.  slowly  in  neu- 
tral aq.  solution,  rapidly  in  acid  aq.  solution; 


326 


CYANIDE,  POTASSIUM  ZINC 


insol.  in  alcohol.  (Locke,  Am.  Ch.  J.  1898, 
20.  601.) 

K4V(CN)3+3H2O.    Sol.  in  H2O. 

Insol.  in  alcohol  and  ether.  (Petersen,  Z. 
anorg.  1904,  38.  345.) 

Potassium  zinc  cyanide,  2KCN,  Zn(CN)2. 

100  pts.  H2O  dissolve  11  pts.  at  20°. 
(Sharwood,  Eng.  Min.  J.  1904,  77.  845.) 

Potassium  cyanide  molybdenum  dioxide, 
4KCN,  MoO2+5H2O. 

Sol.  in  H2O.  Insol.  in  alcohol.  (Hof- 
mann, Z.  anorg.  1896,  12.  287.) 

+6H2O.       "  Potassium    dioxotetracyan- 
omolybdate." 

Very  sol.  in  H2O.  (Winkler,  Dissert. 
1909.) 

+8H2O.  (Rosenheim,  Kohn  and  Gar- 
funkel,  Z.  anorg.  1910,  65.  174.) 

+  10H2O.  Decomp.  by  cone.  HC1,  HNO3 
and  H2S04. 

Not  acted  upon  by  cold  dil.  acids,  (v.  der 
Heide  and  Hofmann,  Z.  anorg.  1896,  12.  285.) 

5KCN,  MoO2+8H2O.  Sol.  in  H2O.  Insol. 
in  alcohol.  (Kalischer,  Dissert.  1902.) 

Potassium    cyanide     molybdenum    cfaoxide 
hydroxylamine,  4KCN,  MoO2,  NH2OH 
+H20. 
Sol.  in  H2O. 

Decomp.  by  dil.  acids,  (v.  der  Heide  and 
Hofmann,  Z.  anorg.  1896,  12.  282.) 

Potassium  cyanide  molybdenum  sulphide, 
6KCN,  Mo2S3+5H2O. 

Easily  sol.  in  H2O.  Decomp.  by  dil.  aeids. 
(Hofmann,  Z.  anorg.  1896,  12.  289.) 

Very  sol.  in  H2O.  Slowly  decomp.  in  the 
cold  bv  dil.  mineral  acids,  (v.  der  Heide  and 
Hofmann,  Z.  anorg.  1896,  12.  289.) 

Potassium    cyanide    molybdenum    sulpho- 

cyanide,  2KCN,   MoS2(CN)2. 
(Pechard,  C.  R.  1894,  118,  806.) 
5KCN,  Mo3S4(CN)3+7H20.    Sol.  in  H2O. 
Stable  toward  dil.  acids  and  alkalies.    (Hof- 
mann, Z.  anorg.  1896,  12.  289.) 

Potassium  cyanide  molybdenum   sulphoxy- 
cyanide,    4KCN,    Mo2SO(CN)2+4H2O. 
Sol.   in   H2O.     Stable  toward   dil.   acids. 
(Hofmann,  Z.  anorg.  1896,  12.  289.) 

Potassium  cyanide  nitrite,  KCN,  KNO2 


Sol.  in  H2O;  decomp.  slowly  by  H2O/ 
explosive.  (Hofmann,  Z.  anorg.  1895, 10.  260- 
261.) 

Potassium  cyanide  sulphur  dioxide,  KCN 

S02+H20. 

Much  more  sol.  in  hot  than  cold  H2O 
(fitard,  C.  R.  88.  649.) 


KCN,  HCN,  2SO2+3H2O.     Very  si.  sol. 
in  cold  H2O;  decomp.  by  hot  H2O.    (Etard.) 

Rubidium  tungsten  cyanide. 
See  Tungstocyanide,  rubidium. 

Rhodium  cyanide,  Rh(CN)3. 

Ppt.      Not    decomp.    by    acids.      Sol.    in 
KCN+Aq.  .(Martius,  A.  117.  361.) 


Rhodium  cyanide  with  3KCN. 
See  Rhodicyanide,  potassium. 

Ruthenium  cyanide  with  4MCN. 
See  Ruthenocyanide,  M. 


Silver  cyanide,  AgCN. 

$1.  sol.  in  H2O. 

2.2  +  10-4  g.  sol.  in  1  liter  of  H2O  at  19.96°. 
(Bottger,  Z.  phys.  ch.  1903,  46.  603.) 

1  1.  solution  "in  H2O  contains  0.000043  g. 
AgCN  at  17.5°.  (Ab.egg  and  Cox,  Z.  phys. 
Ch.  1903,46.  11.) 

Solubility  in  H2O  at  25°=2.22  +  KH 
mol.  per  1.  (Lucas,  Z.  anorg.  1904,  41. 198.) 

Insol.  in  dil.  acids.  Decomp.  by  cone, 
acids.  Not  sol.  to  any  extent  in  HCN+  Aq. 

Freshly  pptd.  AgCN  is  not  dissolved  by 
cold  dil.  HNO3,  but  is  attacked  by  very  dil. 
HNO3  on  boiling.  From  dry  AgCN  is  dis- 
solved 5%  by  boiling  1  hour  with  1%  HNO3 
+Aq.  Cone.  HNO3  dissolves  more.  (Brunck, 

B.  1901,  34.  1605.) 

Sol.  in  NH4OH+Aq.  Sol.  in  boiling 
KC1,  NaCl,  CaCl2,  BaCl2,  or  MgCl2+Aq,  but 
very  slowly  sol.  therein  at  ord.  temp.  Sol.  in 
Na2S203,K4Fe(CN)6,  (NH4)2CO3,  (NH4)2SO4, 
NH4NO3,  and  NH4  succinate-f  Aq,  and  in 
large  amt.  of  hot  NH4Cl+Aq.  (Wittstein.) 

Sol.  in  KCN,  NaCN,  Ba(CN)2,  Ca(CN)2, 
or  Sr(CN)2+Aq.  Insol.  in  KOH,  or  NaOH 
+Aq.  Sol.  in  cone,  boiling  AgNO3+Aq. 
(Wohler.) 

Sol.  in  431.7  pts.  5%  NH4OH+Aq  (sp. 
gr.  0.998)  at  12°;  in  184.5  pts.  10%  NH4OH+ 
Aq  (sp.  gr.  0.96)  at  18°.  (Longi,  Gazz,  ch. 
it.  13.  87.) 

SI.  sol.  in  Na  citrate +Aq. 

Sol.  in  Hg(NO3)2+Aq. 

1  1.  of  a  3-N  solution  of  AgN03  dissolves 
1.216  g.  AgCN  at  25°.  (Hellwig,  Z.  anorg. 
1900,  26.  177.) 

Very  sol.  in  (NH4)2S2O3+Aq.  (Rosen- 
heim and  Steinhauser,  Z.  anorg.  1900,  25. 
105.) 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  829.) 

SI.  sol.  in  liquid  HF.  (Franklin,  Z.  anorg. 
1905,  46.  2.) 

Abundantly  sol.  in  quinoline  at  60°.    (Varet, 

C.  R.  1893,  116.  60.) 

SI.  sol.  in  ethyl  amine.  (Shinn,  J.  phys. 
Chem.  1907,  11.  538.) 

Insol.  in  methyl  acetate.  (Bezold,  Dissert. 
1906;  Naumann,  B.  1909,  42.  3790);  ethyl 


CYANOGEN 


327 


acetate.     (Hamers,  Dissert.  1906;  Naumann 

B.  1910,  43.  314.) 

Silver  hydrogen  cyanide,  AgCN,  HCN. 
(Euler,  B.  1903,  36.  1859.) 

Silver  sodium  cyanide,  AgCN,  NaCN. 

Sol.  in  5  pts.  H2O  at  20°  and  in  much  less 
hot  H2O.  Sol.  in  24  pts.  85%  alcohol  at 
20°.  (Baup,  A.  ch.  (3)  63.  -468.) 

Silver  thallous  cyanide,  AgCN,  T1CN. 

Easily  sol.  in  H20.  100  pts.  H2O  dissolve 
4.7  pts.  at  0°,  and  7.4  pts.  at  16°.  (Fron- 
muller,  B.  11.  92.) 

Silver  tungsten  cyanide. 
See  Tungstocyanide,  silver. 

Silver  cyanide  ammonia,  AgCN,  NH3. 
Efflorescent.     Decomp.  on  air. 
Very  sol.  in  ammonia  at  -10°.     (Joannis, 

C.  R.  1894,  118.  1151.) 

Silver  cyanide  hydrazine,  AgCN,  N2H4. 

Decomp.  in  the  air. 

Decomp.  by  H2O.  (Franzen,  Z.  anorg. 
1911,  70.  153.) 

Silver  cyanide  nitrate,  2AgCN,  AgNO3. 
Decomp.  by  H20. 

Sodium  cyanide,  NaCN. 

Sol.  in  H20  and  75%  alcohol. 

+  >iH2O,  and  2H20.  Very  sol.  in  H2O;  si. 
sol.  in  alcohol.  (Joannis,  A.  ch.  (5)  26.  484.) 

Sodium  tungsten  cyanide. 
See  Tungstocyanide,  sodium. 

Sodium    zinc    cyanide,    NaCN,    Zn(CN)2  + 


Much  more  sol.  in  H2O  than  the  correspond- 
ing K  Zn  salt.    (Rammelsberg.) 
+8H2O.     (Loebe,  Dissert.  1902.) 

Sodium  cyanide  molybdenum  dioxide, 
4NaCN,  MoO2+6H2O. 

(Winkler,  Dissert.  1909.) 

+14H2O.  Sol.  in  H2O.  (Rosenheim, 
Garfunkel  and  Kohn,  Z.  anorg.  1910,  65.  174.) 

Sodium   cyanide   molybdenum   dioxide   hy- 
droxylamine,   4NaCN,    MoO2,    NH2OH 
+H20. 
As  K  comp.    (Winkler,  Dissert.  1909.) 

Strontium  cyanide,  Sr(CN)2+4H2O. 

Very  unstable;  very  deliquescent,  and  sol. 
in  H2O.  (Joannis,  A.  ch.  (5)  26.  496.) 

Strontium  tungsten  cyanide. 
See  Tungstocyanide,  strontium. 


Strontium    zinc    cyanide,    2Sr(CN)2, 
3Zn(CN)2+H2O. 

Sol.  in  H2O  and  alcohol.  (Loebe,  Dissert. 
1902.) 

Thallous  cyanide,  T1CN. 

100  pts.  H2O  dissolve  16.8  pts.  at  28.5°. 
(Fronmuller,  B.  6.  1178.) 

Thallothallic    cyanide,    T12(CN)4  =  T1CN, 

T1(CN)3. 

Easily  sol.  in  H2O. 

100  pts.  H2O  dissolve  27.3  pts.  at  30°,  15.3 
pts.  at  12°,  9.7  pts.  at  0°.  (Fronmuller,  B.  11. 
92.) 

Thallous  tungsten  cyanide. 
See  Tungstocyanide,  thallous. 

Thallous  zinc  cyanide,  2T1CN,  Zn(CN)2. 

Easily  sol.  in  H2O.  100  pts.  H20  dissolve 
8.7  pts.  at  0°;  15.2  pts.  at  14°;  and  29.6  pts. 
at  31°.  (Fronmuller,  B.  11.  92.) 

Tungsten  cyanide  with  MCN. 
See  Tungstocyanide,  M. 

Zinc  cyanide,  Zn(CN)2. 

Insol.  in  H2O  and  alcohol.  Sol.  in  alkalies. 
Easily  sol.  in  KCN+Aq.  Sol.  in  hot  NH4 
salts +Aq.  (Wittstein.) 

Easily  sol.  in   (NH4)2CO3+Aq.     (Gore.) 

Sol.  in  KOH+Aq.  Solution  is  stable 
when  less  than  1  mol.  Zn(CN)2  to  2  mols. 
KOH  is  present.  When  proportion  is  1:1, 
ZnO2H2  soon  separates. 

Sol.  in  dil.  KCN+Aq.  (Sharwood,  J. 
Am.  Chem.  Soc.  1903,  26.  587.) 

SI.  sol.  in  cone.  Zn  salts +Aq.  1  1.  cone. 
Zn(C2H3O2)2+Aq  dissolves  4  g.,  and  1  1. 
cone.  ZnSO4+Aq  dissolves  2  g.  Zn(CN)2. 
Insol.  in  HCN-f  Aq.  Easily  sol.  in  dil. 
acids.  (Joannis.) 

Very  sol.  in  liquid  NH3.  (Franklin,  Am. 
h.  J.  1898,  20.  830.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

Zinc  cyanide  ammonia,  Zn(CN)2,  2NH3. 
Decomp.  on  air.    (Varet,  C.  R.  105.  1070.) 
+H2O.     Decomp.  on  air.     Decomp.  by 

H2O.    Sol.  in  NH4OH+Aq.    (Varet.) 

Zinc  cyanide  cfo'hydrazine,  Zn(CN)2,  2N2H4. 
Decomp.   by  H2O.     (Franzen,   Z.   anorg 
1911,  70.  153.) 

Cyanogen,  CN. 

H2O  absorbs  4*/£  vols.  CN  gas  at  20°.  Alco- 
10!  absorbs  23  vols.,  and  ether  5  vols.  at  the 
same  temperature.  (Gay-Lussac.) 

The  solution  gradually  decomposes,  but 
this  is  prevented  by  traces  of  acids. 


328 


CYCLOTRIBORENE 


0.221  mol.  litre  are  dissolved  in  H2O  at 
0°.  (Naumann,  Z.  Electrochem.  1910,  16. 
177.) 

Oil  of  turpentine  absorbs  5  vols.  (Gay- 
Lussac.)  Absorbed  by  many  essential  oils. 

Very  sol.  in  CuCl2-f  Aq. 

Absorbed  with  decomp.  by  NH4OH+Aq 
and  other  alkaline  liquids. 
k  Absorbed  by  aniline.     (Jacquemain,  C.  R. 
100.  1006.) 

Cyclotriborene,  B3H3. 

Insol.  in  H2O.  (Ramsay  and  Hatfield, 
Proc.  Chem.  Soc.  1901,  17.  152.) 

Decamine  cob al tic  sulphite, 

Co2(NH3)10(S03)3+3H20. 
Sol.  in  H2O.    (Vortmann  and  Magdeburg, 
B.  22.  2636.) 

Decamine  cobaltisulphurous  acid. 

Cobaltic  decamine  cobaltisulphite, 

Co2(NH3)  10(S03)6Co2 +8H20. 
Ppt.     (Vortmann  and  Magdeburg,  B.  22. 
2635.) 

Sodium  decamine  cohaltisulphite, 

Co2(NH3)10(S03Na)6-}-2H20. 
Sol.  in  H2O.     (Vortmann  and  Magdeburg, 
B.  22.  2635.) 

Diamide,  N2H4. 
See  Hydrazine. 

Diamine     chromium     sulphocyanhydric 
acid,  Cr(NH3)12(SCN)3,  HSCN+H2O. 
Sol.  in  H2O.     (Nordenskiold,  Z.  anorg.  1. 
130.) 

Diamine    chromium    cfo'aquo    sulphocyanide. 

Cr(NH3)2(SCN)3+2H20. 
Sol.  in  H2O,  from  which  it  is  pptd.  by  con. 
HCl+Aq.    (Nordenskiold,  Z.  anorg.  1.  137.) 

Ammonium  diamine  chromium  sulphocy- 
anide, Cr(NH3)2(SCN)3,  NH4SCN. 

(Reinecke' s  salt.)  Quite  easily  sol.  in  H2O, 
less  in  alcohol,  and  insol.  in  benzene.  Slowly 
decomp.  by  boiling  H2O  or  dil.  acids.  (Nor- 
denskiold, Z.  anorg.  1.  130.)  . 

+H2O.  Insol.  in  absolute  ether.  (Christen- 
sen,  J.  pr.  (2)  45.  218.) 

Ammonium  diamine  chromium  sulphocyanide 
iodide,  Cr(NH3)2(SCN)3,  NH4SCN,  I. 

Barium ,  [Cr(NH3)2(SCN)3]2, 

Ba(SCN)2. 
Sol.  in  H2O  and  alcohol.    (N.) 


Cadmium  diamine  chromium  sulphocyanide, 

Cd(SCN)2,  [Cr(NH3)2(SCN)3]2+H2O. 
Nearly  insol.  in  cold,  si.  sol.  in  hot  H2O. 
SI.  sol.  in  boiling  alcohol.     (Christensen,  J. 
pr.  (2)  45.  371.) 


Cupric 


[Cr(NH3)2(SCN)< 


Cu(SCN)2, 


Insol.  in  H2O  or  dil.  acids.     (Reinecke,  A. 
126.  116.) 

Ferric 

Fe(SCN)3.     (N.) 

Luteocobaltic , 

Co(NH3)6(SCN)3[Cr(NH3)2(SCN)3]3. 
As  good  as  insol.  in  cold  H2O.    SI.  sol.  in 
hot  H2O  and  alcohol.    (Christensen,  J.  pr.  (2) 
45.  370.) 

Mercuric ,  [Cr(NH3)2(SCN)3]2, 

Hg(SCN)2. 
Insol.  in  H2O.    (N.) 
Insol.  in  H2O  and  dil.  acids.     (Reinecke.) 

Potassium  — = ,  Cr(NH3)2(SCN)3, 

KSCN. 

Properties  as  the  NH4  salt.    (N.) 
Cr(NH3)2(SCN)3,  KSCN,  I.    As  the  NH4 

salt.    (N.) 

Sodium  — ,  NaSCN, 

Cr(NH3)2(SCN)3. 
Sol.  in  H2O,  alcohol,  and  ether.  (Reinecke.) 

Diamine     cobaltic    nitrite     ammonium 
nitrite,  CO(NH3)2(NO2)3,  NH4N02. 
Sol.  inH2O.    (Erdmann.) 

nitrite  lead  nitrite, 

2Co(NH3)2(NO2)3,  Pb(NO2)2. 
Sol.  in  hot  H2O  with  partial  decomp. 

nitrite  mercurous  nitrite, 

2Co(NH3)2(N02)3,  Hg2(N02)2. 
Ppt.    Not  sol.  in  hot  H2O  without  decomp. 

nitrite  potassium  nitrite, 

Co(NH3)2(NO2)3,  KNO2. 
Sol.  in  H2O.     (Erdmann,  J.  pr.  97.  385.) 

nitrite  silver  nitrite, 

Co(NH3)2(N02)3,  AgN02. 

Ppt.    Crystallises  out  of  hot  H2O.    (Erd- 
mann.) 

nitrite  thallium  nitrite, 

Co(NH3)2(NO2)3,  T1NO2. 
Crystallises  out  of  hot  H2O  without  de- 
comp. 


DIDYMIUM  OXIDE 


329 


Dichrocobaltic  carbonate, 

Co(NH3)3(OH)C03  +  l^H20. 
Sol.  in  H2O.    (Vortmann,  B.  15.  1901.) 

Dichrocobaltic  chloride,  Co(NH3)3Cl3+H2O. 

Quite  sol.  in  cold  H2O,  dil.  acids,  cone. 
H2SO4,or  dil.  alcohol. 

From  solution  in  cone.  H2SO4,  the  salt  is 
precipitated  by  much  HCl+Aq.  Composi- 
tion is  Co(NH3)3(OH2)Cl3.  (Jorgensen,  Z. 
anorg.  5.  189.) 

nitrate,  Co(NH3)3(NO3)3+4H2O. 

Deliquescent.  Sol.  in  H20.  More  sol.  in 
dil.  HNO3+Aq  than  praseocobaltic  nitrate. 
(Vortmann,  B.  15.  1897.) 

Anhydrous.  Insol.  in  H2O  as  such,  but 
converted  into  above  salt  thereby.  (Jorgen- 
sen,  Z.  anorg.  5.  186.) 

nitrite,  Co(NH3)3(NO2)3. 

Difficultly  sol.  in  cold,  but  rather  easily  sol. 
in  hot  H2O. 

sulphate,   [Co(NH3)3l2(SO4)3+6H2O. 

Easily  sol.   in  H2O.      (Vortmann,   B.   15. 

1900.) 

sulphite,  [Co(NH3)3]2(SO3)3+H2O. 

Nearly  insol.  in  cold,  slowly  decomp.  by  hot 

H2O.  Decomp.  by  acids  or  KOH+Aq.  Insol. 
in  cold,  sol.  in  warm  NH4OH+Aq.  (Kunzel, 
J.  pr.  (1)  72.  209.)  According  to  Geuther  (A. 
128.  157),  is  a  double  salt — 

[Co(NH3)3]2(S03)3,  Co2(S03)3+2H20. 

Didymium,  Di. 

Slowly  decomp.  by  H2O.  Insol.  in  cold 
cone.  H2SO4.  Sol.  in  dil.  acids. 

Compound  of  two  elements,  neodymium 
and  praseodymium,  (v.  Welsbach.  W.  A. 
B.  92.  317.) 

Didymium  bromide,  DiBr3+6H2O. 

Very  deliquescent,  and  sol.  in  H2O. 
(Cleve.) 

Didymium  nickel  bromide,  2DiBr3,  3NiBr2  + 

18H2O. 

Deliquescent.  Very  sol.  in  H2O.  (Frerichs 
and  Smith,  A.  191.  342.) 

Didymium  zinc  bromide,  DiBr3.  3ZnBr2  + 
12H2O. 

Extremely  deliquescent.  (Cleve,  Bull. 
Soc.  (3)  43.  361.) 

2DiBr3,    3ZnBr2+36H2O.      (F.    and    S.) 

Didymium  chloride,  DiCl3. 

Anhydrous.  Deliquescent.  Sol.  in  H2O 
and  alcohol.  (Marignac.) 

+6H2O.  Deliquescent.  Easily  sol.  in 
H2O  and  alcohol.  (Marignac.) 


Didymium  mercuric  chloride,  2DiCl3, 
9HgCl2+24H20. 

More  sol.  in  H2O  than  the  corresponding 
La  salt.     (Marignac.) 

DiCl3,  4HgCl2+HH2O.    Not  deliquescent. 
Easily  sol.  in  H2O. 

Didymium  stannic  chloride. 
See  Chlorostannate,  didymium. 


Didymium  fluoride, 

Precipitate.     (Cleve.) 

Didymium  hydrogen  fluoride,  2DiF3,  3HF. 
Precipitate.     (Smith.) 
Does  not  exist.    (Cleve.) 

Didymium  potassium  fluoride,  DiF3,  KF  + 

H2O. 

Sol.  in  H2O.    (Brauner,  B.  15.  114.) 
+V3H2O.    As  above.    (B.) 
2DiF3,  3KF+H2O.     As  above.     (B.) 

Didymium  hydroxide,  Di2O6H6. 

Insol.  in  KOH,  or  NaOH+Aq,  but  is  si. 
sol.  in  NH4Cl+Aq.  (Rose.) 

See  also  Di2O3. 

Didymium   pent  hydroxide,    DiO4H3  =  Di205, 

3H2O. 
Precipitate.     (Brauner,  B.  15.  113.) 

Didymium  zinc  iodide,  2DiI3,  3ZnI2+24H2O. 
Very  deliquescent.     (Frerichs  and  Smith.) 

Didymium  oxide,  Di2O3. 

With  H2O  slowly  forms  Di2O6H6. 

Sol.  in  cone.,  or  dil.  mineral  acids  (Marig- 
nac), and  in  acetic  acid  (Hermann).  Sol.  in 
ammonium  salts  +Aq. 

Slightly  more  slowly  sol.  in  cone.  NH4NO3 
+Aq  than  La2O3.  (Damour  and  Deville.) 

A  solution  of  NH4NO3  in  H2O  that  can 
dissolve  2.9  mols.  La2O3  dissolves  1  mol. 
Di2O3.  (Brauner,  B.  15.  114.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329.) 

Didymium  peroxide,  Di409. 

Sol.  in  acids  with  decomp.  (Frerichs,  B. 
7.  799.) 

Not  obtained  by  Cleve.  (B.  11.  910.) 
The  contradictory  statements  concerning 
the  composition  of  Di  peroxide  are  owing  to 
the  fact  that  praseodidymium  is  the  only  one 
of  the  constituents  of  Di  which  easily  forms  a 
peroxide,  (v.  Welsbach.) 

Didymium  peroxide,  Di206. 

Sol.  in  dil.  HNO3,  or  H2SO4+Aq  in  the 
cold  without  evolution  of  gas,  but  gas  is 
evolved  if  treated  with  cone,  acids.  Insol. 
in  HF+Aq.  SI.  sol.  in  cold  NH4NO3+Aq. 
=  Di4O9.  (Cleve.) 


330 


DIDYMIUM  OXYBROMIDE 


Didymium  oxybromide,  DiOBr. 

(Frerichs  and  Smith.) 

Didymium  oxychloride,  DiOCl. 

Anhydrous.      Insol.    in    H2O.      (Smith.) 
+3H2O.     Sol.   in   cold   dil.   HNO3+Aq. 
(Marignac.)     SI.   sol.   in  HCl+Aq.     (Her- 
mann.) 

Didymium  oxysulphide,  Di2O2S. 

Insol.  in  H2O.  Sol.  in  HCl+Aq  without 
residue.  (Marignac.) 

Didymium  sulphide,  Di2S3. 

Insol.  in  H2O.  Decomp.  by  dil.  acids. 
(Marignac,  A.  ch.  (3)  38.  159.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329.) 

Disulphuric  acid,  H2S2O7. 
See  Disulphuric  acid. 

Dithionic  acid   (Hyposulphuric  acid), 

H2S2O6. 

Known  only  in  aqueous  solution,  which  is 
stable  only  when  dil.  Can  be  evaporated  in 
vacuo  until  sp.  gr.  =  1.347,  but  decomp.  upon 
further  evaporation.  (Welter  and  Gay- 
Lussac,  A.  ch.  10.  312.) 

Dithionates. 

All  dithionates  are  sol.  in  H2O. 

Aluminum  dithionate,  A12(S2O6)3+18H2O. 

Extremely  deliquescent.  Easily  sol.  in  H20 
or  absolute  alcohol.  (Kliiss,  A.  246. 218.) 

Aluminum  ammonium  dithionate. 

A12(S206)3,  (NH4)2S206+27H20. 
SI.  deliquescent.    Sol.  in  H2O.    (Kliiss,  A. 
246.  303.) 

Ammonium  dithionate,   (NH4)2S2O6. 

Very  sol.  in  H2O.  Sol.  in  0.79  pt.  H2O  at 
16°,  with  reduction  of  temp.-  Not  decomp.  on 
boiling.  Insol.  in  absolute  alcohol.  (Heeren, 
Pogg.  7. 172.) 

Contains  }/£H20.  Sol.  in  0.56  pt.  H2O  at 
19°.  (Kliiss,  A.  246. 194.) 

Ammonium  cadmium  dithionate, 

2(NH4)2S2O6,  CdS2O6+4^H2O. 
Sol.  in  H2O.     (Kliiss,  A.  246.  298.) 

Ammonium  cobalt  dithionate,  9(NH4)2S2Ofi, 

2CoS206  +  16^H20. 
Sol.  in  H2O.     (Kliiss.) 

Ammonium    cupric    dithionate,    (NH4)2S2O6, 

2CuS2O6+8H2O. 
Sol.  in  H2O. 


Ammonium  ferrous  dithionate,  3(NH4)2S2O6, 

Fe2S2O6+6H2O. 

Sol.  iii  H20.    (Kliiss,  A.  246.  300.) 
9(NH4)2S2O6,     2Fe2S2O6  +  16^H20.      Sol. 

in  H20.     (Kliiss.) 

Ammonium  manganous  dithionate, 

9(NH4)2S2O6,  2MnS2O6. 
Sol.  in  H2O.    (Kliiss,  A.  246.  301.) 

Ammonium  nickel  dithionate,  9(NH4)2S2O6, 

2NiS2O6  +  16^H2O. 
Sol.inH2O.    (Kliiss.) 

Ammonium    zinc    dithionate,    5(NH4)2S206, 

ZnS2O6+9H2O. 
Easily  sol.  in  H2O.    (Kliiss,  A.  246.  296.) 

9(NH4)2S2OC,  2ZnS2O6+16MH2O.  Easily 
sol.  in  H2O.  (Kliiss.) 

Ammonium  dithionate  chloride,  (NH4)2S2O6, 

NH4C1. 

Sol.  in  H2O.  (Fock  and  Kliiss,  B.  24. 
3017.) 

Barium  dithionate,  BaS2O6+2H2O. 

Not  efflorescent.  Sol.  in  7.17  pts.  H2O  at 
8°,  4.04  pts.  at  18°,  and  1.1  pts.  H2O  at  100°. 

Insol.  in  alcohol.     (Gay-Lussac,  Heeren.) 

Sol.  in  0.994  pt.  H2O  at  102°,  the  boiling- 
point  of  the  sat.  solution.  (Baker,  Bull. 
Soc.  (2)  44.  166.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

+4H2O.    Very  efflorescent.    (Heeren.) 

Barium  magnesium  dithionate,  BaMg(S2O6)2 

+4H2O. 
Sol.  in  H2O.    (Schiff,  A.  118.  97.) 

Barium  rubidium   dithionate,   BaRb4(S2O6)3 

+H20. 

Sol.  in  H2O.  Solubility  is  diminished  by 
presence  of  excess  of  Rb2SO4,  but  increased  by 
BaS2O6.  (Bodlander,  Chem.  Ztg.  14.  1140.) 

Barium  sodium  dithionate,  BaNa4(S2O6)3  + 
4H2O. 

Sol.  in  H2O  .  Decomp.  by  recrystallisation. 
(Kraut,  A.  118.  95.) 

+6H2O.    (Schiff.) 

Barium  dithionate  chloride,  BaS2O6,  BaCl2  + 

4H2O. 
(Fock  and  Kliiss,  B.  23.  3001.) 

Bismuth  dithionate,  basic,  Bi2O3,  S2O5  + 
+5H2O. 

Efflorescent.  Insol.  in  H2O,  but  decomp. 
thereby  into  the  following  salt.  Easily  sol. 
in  dil.  acids,  especially  HCl+Aq.  (Kluss,  A. 
246.  183.) 

4Bi2O3,  3S2O6+5H2O.  Insol.  in  H2O.  Sol. 
in  dil.  acids.  (Kliiss.) 


DITHIONATE,  MANGANOUS 


331 


Cadmium  dithionate. 

Deliquescent  in  moist  air;  very  sol.  in  H2O. 
(Heeren,  Pogg.  7.  183.) 

Cadmium     dithionate     ammonia,     CdS2Oe, 

Decomp.  by  alcohol;  sol.  in  NH4OH+Aq, 
but  decomp.  on  heating.  (Rammelsberg, 
Pogg.  68.  298.) 

Caesium  dithionate,  Cs2S2O6. 

Easily  sol.  in  H2O.  (Chabrie,  C.  R.  1901, 
133.  297.) 

Calcium  dithionate,  CaS2Oe+4H2O. 

Sol.  in  2.46  pts.  H2O  at  19°;  0.8  pt.  at  100.° 
Insol.  in  alcohol.  (Heeren,  Pogg.  7. 178.) 

Insol.  in  acetone.  (Naumann.  B.  1904. 
37.  4329.) 

Cerous    dithionate,    Ce2(S2O6)3+24H2O. 
Very  sol.  in  H2O.    (Jolin.) 
+3,  and5H2O.    (Wyrouboff.) 

Chromic  dithionate,  Cr2(S2O6)3+18H2O. 

Sol.  in  H2O  and  alcohol.  (Kltiss,  A.  246. 
189.) 

3O2O3,  4S206+24H2O.  Easily  sol.  in  H2O 
or  alcohol.  Insol.  in  ether.  (Kliiss.) 

Cobaltous   dithionate,   CoS2O6+6H2O. 

Not  deliquescent.  Very  sol.  in  H2O. 
(Heeren.) 

+8H2O.  Sol.  in  0.49  pt.  H2O  at  19°.  Sol. 
in  absolute  alcohol.  (Kliiss,  A.  246.  203.) 

Cupric  dithionate  basic,  4CuO,  S2O6+4H2O. 

Very  sl^  sol.  in  H2O.  (Heeren,  Pogg.  7. 
18.) 

Insol.  in  H2O;  easily  sol.  in  dil.  acids. 
(Kliiss,  A.  246.  208.) 

+3H2O.  Insol.  in  H20  and  NaC2H3O2+ 
Aq;  sol.  in  traces  in  cone.  CuS2Of+Aq. 
Easily  sol.  in  dil.  acids,  even  HC2H3O2,  or 
H2S2O6+Aq.  (Kliiss.) 

Cupric  dithionate,  CuS2O6+4H2O. 

Not  efflorescent.  Very  sol.  in  H2O.  Insol. 
in  alcohol.  (Heeren.) 

H-5H2O.  (Efflorescent.  Sol.  in  0.64  pt. 
H2Oatl8.5.°  (Kliiss,  A.  246.  204.) 

Cupric  dithionate  ammonia,  CuS2O6,  4NH3. 

Difficultly  sol.  in  cold  H2O,  moderately  sol. 
in  H2O  at  40°.  Decomp.  by  much  H2O  or  by 
heating  the  solution  above  60°.  Decomp.  by 
HCl+Aq.  (Heeren.) 

Can  be  recryst.  from  NH4OH+Aq. 

Sol.  in  liquid  NH3.  (Horn,  Am.  Ch.  J. 
1908,  39.  213.) 

CuS2O6,  9NH3.  Decomp.  at  ord.  temp, 
in  the  air. 

Insol.  in  liquid  NH3.  (Horn,  Am.  Ch.  J. 
1908,  39.  213.) 


Didymium    dithionate,    Di2(S2O6)3+24H2O. 
Extremely  sol.  in  H2O.     (Cleve.) 

Erbium    dithionate,    Er2(S2O6)3  +  18H2O. 

Very  sol.  in  H2O  or  alcohol;  insol.  in  ether. 
(Hoglund.) 

Glucinum  dithonate,  basic,  5G1O,  2S2O6  + 

14H20. 

Easily  sol.  in  H2O  and  absolute  alcohol. 
(Kliiss,  A.  246.  196.) 

Iron  (ferrous)  dithionate,  FeS2O6+5H20. 

Very  sol.  in  H2O.  Insol.  in  alcohol.  De- 
comp. in  aqueous  solution  into  FeSO4  by 
boiling.  (Heeren,  Pogg.  7.  181.) 

+7H2O.  Sol.  in  0.59  pt.  H2O  at  18.5°. 
(Kliiss,  A.  246.  198.) 

Iron  (ferric)  dithionate,  basic,  8Fe2O3,  S2O6  + 

20H2O. 
Insol.  in  H20  or  alcohol.    Very  si.  sol.  in 

H2S2O6+Aq;    easily    sol.    in    HCl+Aq. 

(Heeren.) 

Contains  14H2O.     (Kliiss,  A.  246.  200.) 
3Fe2O3,     S208+8H2O.       Insol.     in    H2O. 

Easily  sol.  in  acids.    (Kliiss,  A.  246.  201.) 

Lanthanum    dithionate,    La2(S2O6)8+16H2O, 

and  24H2O. 
Sol.  in  H2O.    (Cleve.) 

Lead  dithionate,  basic,  2PbO,  S2O6+2H2O. 

Very  difficultly  sol.  in  H20.  (Heeren, 
Pogg.  7.  171.) 

lOPbO,  S2O6+2H2O.  SI.  sol.  in  H2O. 
(Heeren.) 

Lead  dithionate,  PbS2O6+4H2O. 

Easily  sol.  in  H2O.    (Heern.) 

Sol.  in  0.869  pt.  H2O  at  20.5°.  (Baker, 
C.  N.  36.  203.) 

Lead    strontium    dithionate,    (Pb,Sr)S2O6+ 
4H20. 
(Rammelsberg.) 


Lithium  dithionate,  Li2S2O6+2H2O. 

SI.  deliquescent,  and  easily  sol. 

Insol.  in  alcohol.     (Rammelsberg.) 


Magnesium   dithionate,   MgS2O6+6H20. 

Sol.  in  0.85  pt.  H2O  at  13°.  Solution  can 
be  boiled  without  decomp.  (Heeren,  Pogg. 
7.  179.) 

Sol.  in  0.692  pt.  H2O  at  17°.  (Baker,  C.  N. 
36.  203.) 

Manganous   dithionate,   MnS2O6+3H2O. 
Sol.  in  H2O.    (Kraut,  A.  118.  98.) 
+6H2O.   Efflorescent.   Sol.inH2O.    (Mar- 

gnac,  J.  B.  1855.  380.) 


332 


DITHIONATE,  MERCUROUS 


Mercurous  dithionate,  Hg2S2O6. 

SI.  sol.  in  cold,  decomp.  by  hot  H20. 
(Rammelsberg.) 

Mercuric    dithionate,    basic,    5HgO,    2S2O5. 
SI.    sol.    in   cold,    decomp.    by   hot   H2O. 
Easily  sol.  in  HNO3+Aq.     (Rammelsberg, 
Pogg.  59.  472.) 

Mercuric    dithionate,    HgS2O6+6H2O. 

Decomp.  by  H2O  or  on  standing.  (Kluss, 
A.  246.  216.) 

Nickel  dithionate,  NiS2O6+6H2O. 

Sol.  inH2O.    (Topsoe.) 

Sol.  in  0.897  pt.  H2O  at  12°.  (Baker,  C.  N. 
36.  203.) 

Nickel  dithionate  ammonia,  NiS2O6,  6NH3. 

Can  be  recryst.  from  warm  NH4OH+Aq. 

Decomp.  by  H2Q.  (Rammelsberg,  Pogg. 
58.  295.) 

Nickel  dithionate  hydrazine,  NiS200, 
3N2H4. 

Unstable. 

Sol.  in  NH4OH+Aq.  (Franzen,  Z.  anorg. 
1908,  60.  267.) 

Potassium  dithionate,  K2S2O6. 

Not  deliquescent.  Sol.  in  16.5  pts.  H2O  at 
16°,  and  1.58  pts.  at  100°.  Insol.  in  alcohol. 
(Heeren.) 

Sol.  in  2.65  pts.  H2O  at  16°.     (Dumas.) 

Sol.  in  16.5  pts.  H2O  at  16°;  in  1.58  pts. 
boiling  H2O. 

Insol.  in  alcohol.  (Heeren,  Pogg.  1826,  7. 
72.) 

Praseodymium       dithionate,       Pr2(S2Oc)3+ 

12H2O. 

Deliquescent;  very  sol.  in  H2O.  (von 
Schule,  Z.  anorg.  1898,  18.  361.) 

Rubidium  dithionate,  Rb2S2O6. 

Sol.  in  H20.     (Topsoe  and  Christiansen:) 

Ruthenium  dithionate,  RuS2O6. 

Ppt.  from  aq.  sol.  by  alcohol.  (Antony, 
Gazz.  ch.  it.  1898,  28.  139-142.) 

Silver  dithionate,  Ag2S2O6 +2H2O. 

Sol.  in  2  pts.  H2O  at  16°.  Sol.  in  NH4OH  + 
Aq.  (Heeren,  Pogg.  7.  191.) 

Silver  sodium   dithionate,  AgS2O6,   Na2S2O6 

+4H20. 
Sol.  in  H2O.    (Kraut,  A.  118.  96.) 

Silver  dithionate  ammonia,  Ag2S2O6,  4NH3. 

Sol.  in  H2O  without  decomp.  (Rammels- 
berg, Pogg.  58.  298.) 


Sodium  dithionate,  Na2S2O6+2H2O. 

89!.  in  2.1  pts.  H2O  at  16°,  and  in  1.1  pts. 
boiling  H2O.  Insol.  in  alcohol. 

Fuming  HCl+Aq  precipitates  the  salt 
from  aqueous  solution.  (Heeren,  Pogg.  7. 
76.) 

+6H2O.     (Kraut,  A.  117.  97.) 

Strontium  dithionate,  SrS2O6+4H2O. 

Sol.  in  4.5  pts.  H2O  at  16°,  1.5  pts.  boiling 
H2O.  Insol.  in  alcohol.  (Heeren,  Pogg.  7. 
177.) 

Thallous  dithionate,  T12S2O6. 

Very  easily  sol.  in  H2O.     (Werther.) 

Thallous     dithionate     sulphate,     3T12S2O6, 

T12S04. 

Sol.  in  H2O.  (Wyrouboff,  Ann.  Phys. 
Beibl.  8.  802.) 

Thorium  dithionate,  Th(S2O6)2+4H2O   (?). 
Very  unstable.     (Kluss,  A.  246.  188.) 

Tin  (stannous)  dithionate,  SnS2Oe. 

Known  only  in  solution. 

8SnO,  S2O5+9H2O.  Insol.  in  H2O.  Sol. 
in  dil.  acids,  even  dithionic  acid+Aq.  (Kluss, 
A.  246.  186.) 

Uranous  dithionate,  6UO2,  S2O5  +  10H2O. 

Insol.  in  H2O;  sol.  in  warm  HCl+Aq. 
(Kluss,  A.  246.  191.) 

7UO2,  S2O5+8H2O.    As  above. 

8UO2,  S2O6+21H2O.     As  above. 

Zh'vanadyl-  dithionate,  (VO2)2S2O6.* 
Sol.  in  H2O.    (Bevan,  C.  N.  38.  294.) 

Yttrium  dithionate,  Y2(S2O6)3  +  1SH2O. 

Not  deliquescent.  Easily  sol.  in  H2O,  but 
difficultly  sol.  in  alcohol.  Insol.  in  ether. 
(Cleve,  Bull.  Soc.  (2)  21.  344.) 

Zinc  dithionate,  ZnS2O6+6H2O. 

Very  sol.  in  H2O;  decomp.  on  boiling. 
(Heeren,  Pogg.  7.  183.) 

Zinc  dithionate  ammonia,  ZnS2Oe,  4NH3. 

Decomp.  with  H2O;  sol.  in  warm,  less  sol. 
in  cold  NH4OH+Aq.  (Rammelsberg,  Pogg. 
58.  297.) 

+H2O.  Ppt.  (Ephraim,  B.  1915,  48. 
640.) 

Dysprosium,  Dy. 

(Lecoq  de  Boisbaudran,  C.  R.  102.  1005.) 

Dysprosium  chloride,  DyCl3+6H2O. 

Deliquescent,  sol.  in  H2O.  (Urbain,  C.  R  . 
1908,  146.  129.) 


FERRATE,  SODIUM 


333 


Europium. 

Europium  chloride,  EuCl2. 

Sol.  in  H2O.  Stable  in  very  dil.  aqueous 
solution,  but  decomp.  when  the  solution  is 
concentrated  at  100°.  (Urbain,  C.  R.  1911, 
163.  1157.) 

Erbium,  Er. 

Decomposes  H2O.    (Hoglund.) 

The  so-called  element  "erbium''  can  be 
further  decomp.  into  simple  substances. 
(Kriiss,  Z.  anorg.  3.  353.) 

Erbium  bromide,  ErBr3+9H2O. 
Very  deliquescent. 

Erbium  chloride,  ErCl3+6H2O. 

Deliquescent.  Sol.  in  H2O  and  alcohol. 
(Hoglund.) 

Erbium  mercuric  chloride,  ErCl3,  5HgCl2  + 


Deliquescent.    (Cleve.) 

Erbium  fluoride,  ErF3. 

Insol.  in  H2O.  Very  si.  sol.  in  HF+Aq. 
(Hoglund,  Bull.  Soc.  (2)  18.  193.) 

Erbium  hydroxide,  Er2O(OH)4. 

Insol.  in  KOH,  or  NaOH+Aq. 

Easily  sol.  in  acids.  Decomp.  ammonium 
salts  by  boiling  therewith. 

Erbium  iodide,  ErI3. 

Very  deliquescent.  Very  sol.  in  H20  and 
alcohol.  Insol.  in  ether.  (Hoglund.) 

Erbium  oxide,  Er2O3. 

Difficultly  but  completely  sol.  in  warm 
HNOa,  H2SO4,  or  HCl+Aq.  Decomp.  NH4 
salts  by  boiling  therewith. 

Erbium  peroxide,  Er2O5. 

Precipitate.  (Cleve,  Bull.  Soc.  (2)  43. 
53.) 

Erbium  sulphide. 

Decomp.  in  moist  air  and  with  acids. 

Erythrochromium  bromide, 

HOCr2(NH3)10Br5+H2O. 
Very  easily  sol.  in  H2O.    Insol.  in  HBr  + 
Aq.     Sol.  in  NH4OH+Aq.     (Jorgensen,  J. 
pr.  (2)  25.  398.) 

-  bromide,  basic,  HOCr2(NH3)io(OH)Br4 

+H20. 
Very  sol.  in  H2O.    (Jorgensen.) 

-  chloroiodide,  HOCr2(NH3)1oClI4+H2O. 
Sol.  in  H2O  and  in  alcohol.     (Jorgensen.) 


Erythrochromium  chloroplatinate, 

[HOCr2fNH3)10]2(PtCl6)6  +  10H20. 
Nearly  insol.  in  H2O.     (Jorgensen.) 

dithionate,  basic, 

HOCr2(NH3)10(S2Oe)2(OH)+2H2O. 
Insol.   in  H2O.     Easily  sol.   in  very  dil. 
HNO3,  HBr,  HCl+Aq.    Sol.  in  cone.  NH4C1 
+Aq.     (Jorgensen.) 

-nitrate,  HOCr2(NH3)10(NO3)5+H2O. 

Easily  sol.  in  H2O.  Insol.  in  dil.  HNO3+ 
Aq.  Sol.  in  cone.  HNO3  with  decomp.  Very 
sol.  in  dil.  NH4OH+Aq.  Insol.  in  alcohol. 
(Jorgensen.) 

nitrater  basic,  HOCr2(NH3)10(NO3)4OH 

+3^H20. 
Sol.  in  cold  H2O.     (Jorgensen.) 

-  sulphate,  [HOCr2(NH3)10]2(SO4)5. 
Nearly  insol.  in  H2O.     (Jorgensen.) 

Tdraferriammonium,  Fe2N. 
See  Iron  nitride. 

Ferric  acid. 

Barium  ferrate,  BaFeO4+H2O. 

Ppt.  Can  be  boiled  for  some  time  with  H2O 
without  decomp.  Decomp.  by  mineral  acids. 
Sol.  in  dil.  acetic  acid.  (Fremy,  A.  ch.  (3) 
12.  373.) 

Insol.  in  H2O;  not  readily  acted  upon  by 
acids  when  dry.  (Rosen,  J.  Am.  Chem. 
Soc.  1895,  17.  766.) 

Ppt.  Easily  decomp.  by  acids.  (Moeser, 
Arch.  Pharm.  1895,  233.  526.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Calcium  ferrate,  CaF2O4. 

Sol.  in  H2O.  (Resell,  J.  Am.  Chem.  Soc. 
1895,  17.  760-69.) 

Potassium  ferrate,  K2FeO4. 

Very  deliquescent.  Easily  sol.  in  cold  H2O 
with  evolution  of  much  heat.  Decomp.  by 
standing  or  warming.  Decomp.  by  acids  or 
alkalies.  (Fremy,  A.  ch.  (3)  12.  369.) 

Sol.  in  H2O;  insol.  in  alcohol.  (Moeser, 
Arch.  Pharm.  1895,  233.  524.) 

Quickly  decomp.  by  potassium  tartrate  or 
racemate,  sugar,  or  albumen  without  separa- 
tion of  Fe2O6H6,  by  alcohol  with  separation 
of  Fe2O6H6.  Potassium  oxalate,  acetate, 
formate,  and  benzoate,  also  citrate  decomp. 
much  more  slowly.  Insol.  in  cone.  KOH  + 
Aq.  (Wackenroder,  A.  33.  41.) 

Sodium  ferrate,  Na2FeO4. 

Sol.  in  H2O  and  in  cone.  NaOH+Aq. 
(Fremy,  1.  c.) 


334 


FERRATE,  STRONTIUM 


Strontium  ferrate,  SrFeO4. 

SI.  sol.  in  H2O  by  which  it  is  decomp. 

Decomp.  by  acids. 

Sol.  in  aqueous  solutions  of  Na  aud  K  salts 
with  partial  decomp. 

Insol.  in  sat.  SrBr2+Aq.,  alcohol  and  ether. 
(Eidmann,  B.  1903,  36,  2290.) 

Ferricomolybdic  acid. 

Ammonium     ferricomolybdate,     3(NH4)aO, 

Fe2O3,  12MoO3  +  19H2O. 
Ppt.     (Hall,  J.  Am.  Chem.  Soc.  1907,  29. 
697.) 

Ferricyanhydric  acid, 

H3Fe(CN)3,    (or    HeFe2(CN)12). 

Easily  sol.  in  H20  or  alcohol.  Solution 
decomposes  slowly  by  standing,  more  rapidly 
by  heating.  Insol.  in  ether. 

Ferricyanides. 

The  alkali,  and  alkaline-earth  ferricyanides 
are  sol.  in  H2O;  the  others  are  insol.  The 
ferricyanides  of  metals,  the  oxides  of  which 
are  sol.  in  NH4OH,  or  KOH+Aq,  are  them- 
selves sol.  in  those  reagents. 

Ammonium  ferricyanide,   (NH4)3Fe(CN)6  + 

3H20. 

Permanent.  Readily  sol.  in  H2O  (and 
alcohol?). 

Ammonium  ferrous  ferricyanide, 

NH4FeFe(CN)6  + 1 HH2O. 
Sol.  in  H2O  and  not  pptd.  by  alcohol  from 
aqueous  solution.    More  stable  than  the  cor- 
responding K  salt. 

Ammonium  lead  ferricyanide, 
NH4PbFe(CN)6+3H2O. 

Ammonium  potassium  ferricyanide, 

(NH4)2KFe(CN)6. 

Sol.  in  H2O.  (Schaller,  Bull.  Soc.  (2)  1. 
275.) 

Barium    ferricyanide,     Ba3[Fe(CN)6]2+ 

20H2O. 

Easily  sol.  in  H2O;  insol.  in  alcohol. 
(Schuler,  W.  A.  B.  77.  692.) 

Barium  potassium  ferricyanide,  BaKFe(CN)6 

+3H2O. 

Permanent.  Easily  sol.  in  H2O,  less  in 
alcohol. 

Barium  ferricyanide  bromide,  Ba3[Fe(CN)6]2, 

2BaBr2+20H2O. 

Easily  sol.  in  H2O.  Boiling  alcohol  does 
not  dissolve  out  BaBr2.  (Rammelsberg,  J. 
pr.  (2)  39.  463.) 


Bismuth  ferricyanide,  Bi3[Fe(CN")6]5. 

Insol.  in  H2O,  but  decomp.  by  boiling 
therewith.  (Muir,  Chem.  Soc.  32.  40.) 

Cadmium  ferricyanide  ammonia, 

Cd3[Fe(CN)6]2,  6NH3+3H20. 
Effloresces  to  form — 

Cd3[Fe(CN)]2,  4NH3+2H20.  Insol.  in 
H2O.  (WyroubofT,  A.  he.  (5)  10.  413.) 

Calcium     ferricyanide,     Ca3[Fe(CN)6]2+10, 

or  12H20. 
Deliquescent.    Sol.  in  H2O  and  dil.  alcohol. 

Calcium  potassium  ferricyanide, 

CaKFe(CN)5. 
Sol.  in  H2O. 

Cerous  ferricyanide,  CeFe(CN)6+4H2O. 
Sol.  in  H2O;  easily  decomp.    (Jolin.) 

Chromic  ferricyanide  (?). 
Ppt. 

Cobaltous  ferricyanide,  Co3[Fe(CN)6]2. 

Insol.  in  H2O  and  HCl+Aq.  Sol.  in 
NH4OH+Aq. 

Cobaltous  ferricyanide  ammonia, 

Co3[Fe(CN)6]2,  4NH3+6H20. 

Cobaltic  ferricyanide  ammonia. 

See  Luteo,-  purpureo,-  etc.  cobaltic  fern- 
cyanide. 

Cuprous  ferricyanide,  (Cu2)3[Fe(CN)6]2. 

Sol.  in  NH4OH+Aq;  insol.  in  NH4  salts-f- 
Aq.  (Wittstein.) 

Cupric  ferricyanide,   Cu3[Fe(CN)6]2. 

Insol.  in  H2O  or  NH4  salts +Aq.  Sol.  in 
NH4OH,  and  (NH4)2CO3+Aq.  (Wittstein.) 

Insol.  in  HCl+Aq. 

Iron  (ferrous)  ferricyanide,  Fe3[Fe(CN)e]2  + 

zH2O. 

(TurnbuWs  blue.)  Properties  as  ferric 
ferrocyanide  (Prussian  blue),  with  which  it  is 
perhaps  identical.  (Gintl,  Z.  anal.  21.  110.) 

Iron   (ferrosoferric)   ferricyanide, 

Fe13(CN)36  =FeI4IFeII[Fe(CN)6]6. 

(Prussian  green.)  Insol.  in  H2O  or  cone. 
HCl+Aq,  but  slowly  decomp.  by  boiling 
therewith. 

Fe3(CN)8+4H2p  =  FeIJFeII2I[Fe(CN)f]4+ 
12H2O.     Properties   as   above.      (Reynolds, 
Chem.  Soc.  64.  767.) 

Iron  (ferrous)  potassium  ferricyanide, 

KFe2(CN)6=KFeFe(CN)6+4,  or  3H2O. 
(Soluble  Prussian  blue.)    Sol.  in  H2O,  but 
insol.  in  salts+Aq  or  alcohol. 


FERRICYANIDE,  POTASSIUM 


335 


Salt  of  the  same  composition,  called  "Wil- 
liamson's blue,"  is  insol.  in  H2O. 

Lead    ferricyanide,     basic,     Pb3[Fe(CN)6]2, 

3Pb02H2  +  llH20. 
(Schuler.) 

Lead    ferricyanide,    Pb3[Fe(CN)6]2+16H2O. 

SI.  sol.  in  H2O;  more  sol.  in  hot,  than  cold 
H2O,  but  decomp.  on  boiling.  (Gmelin.) 

+4H2O.  Easily  sol.  in  H2O;  si.  sol.  in 
alcohol.  (Schuler,  W.  A.  B.  77.  692.) 

Lead  potassium  ferricyanide,  PbKFe(CN)e 
+3H2O. 

Sol.  in  4.75  pts.  H2O  at  16°,  and  the  solu- 
tion decomp.  on  standing.  (Schuler.) 

+  1^H2O.  Efflorescent.  Much  more  sol. 
in  H2O  than  the  Pb  salt.  Insol.  in  alcohol. 
(Wyrouboff.) 

Lead    ferricyanide    nitrate,    Pb3[Fe(CN)B]2, 

Pb(NO3)2+12H2O. 

Sol.  in  13.31  pts.  H2O  at  16°.     (Schuler.) 
+11H2O.    (Joannis,  A.  ch.  (5)  26.  528.) 

Magnesium  ferricyanide,   Mg3[Fe(CN)6]2. 
Sol.  in  H20. 

Magnesium  potassium  ferricyanide, 

MgKFe(CN)6. 
(Reindel,  J.  pr.  103.  166.) 

Manganous  ferricyanide,  Mn3[Fe(CN)6]2. 

Insol.  in  H2O,  acids,  NH4OH,  or  NH4  salts 
+Aq. 

Mercurous  ferricyanide,  Hg3Fe(CN)6. 

Ppt.  (Fernekes,  J.  Am.  Chem.  Soc.  1906, 
28.  604.) 

Mercuric  femcyanide,  Hg3[Fe(CN)6]2. 

Very  sol.  in  H2O.  Solution  quickly  decomp. 
(Fernekes,  J.  Am.  Chem.  Soc.  1906,  28.  603.) 

Nickel  ferricyanide  ammonia,  Ni3[Fe(CN)6]2, 

4NH3+H2O. 

Sol.  in  NH4OH+Aq.  (Reynoso,  A.  ch.(3) 
30.  254.) 

Nickel  ferricyanide,  Ni3[Fe(CN)6]2(?). 
Ppt.    Insol.  in  HCl+Aq. 

Potassium    ferricyanide,     K3Fe(CN)6,     (or 

K6Fe2(CN)12). 
Permanent.    Easily  sol.  in  H2O. 

'100  pts.  H2O  dissolve  pts.  K3Fe(CN)6  at  t°. 


t° 

Pts. 
salt 

t° 

Pts. 

salt 

t° 

Pts. 
salt 

4.4 
10 

33.0 
36.6 

15.6 

37.8 

40.8 

58.8 

100 
104.4 

77.5 

82.6 

(Wallace,  Chem.  Soc.  7.  80.) 


100  pts.  H2O  at  13°  dissolve  38  pts.,  and  the 
solution  has  sp.  gr.  =  1.1630.  (Schiff,  A.  113. 
350.) 

1  1.  sat.  solution  in  H2O  at  25°  contains 
385.5  g.  K3Fe(CN)6.  (Grube,  Z.  Electrochem. 
1914,  20.  342.) 

Sp.  gr.  of  K3Fe(CN)6+Aq  at  13°. 


% 

salt 

Sp.  gr. 

% 

salt 

Sp.  gr. 

SSt 

Sp.  gr. 

1 

1.0051 

11 

1  .  0595 

21 

1  .  1202 

2 

.0103 

12 

1.0653 

22 

1  .  1266 

3 

.0155 

13 

1.0712 

23 

1.1331 

4 

.0208 

14 

1.0771 

24 

1.1396 

5 

.0261 

15 

1.0831 

25 

1.1462 

6 

.0315 

16 

1  .  0891 

26 

1.1529 

7 

.0370 

17 

1.0952 

27 

1.1596 

8 

.0426 

18 

1.1014 

28 

1  .  1664 

9 

1.0482 

19 

1.1076 

29 

1  .  1732 

10 

1.0538 

20 

1.1039 

30 

1.1802 

(Schiff.) 
Sp.  gr.  of  K3Fe(CN)6+Aq  at  25°. 


Concentration  of  K3Fe(CN)6 
+Aq. 

Sp.  gr. 

1  —  normal 

Vr-    ;; 

Vs—       " 

1  .  0574 
1  .  0289 
1.0143 
1.0092 

(Wagner,    Z.   phys.    Ch.    1890,    5.   37.) 

Sat,  K3Fe(CN)6+Aq  boils  at  104.4°. 
(Wallace.) 

1  1.  sat.  solution  at  25°  of  K8Fe(CN)6  + 
K4Fe(CN)6  contains  338.1  g.  K3Fe(CN)6  and 
79.02  g.  K4Fe(CN)6.  (Grube.) 

Solubility  of  K3Fe(CN)6+K4Fe(CN)6  in 
KOH+Aq  at  25°. 


KOH 

Normality 

g.  per  1. 

K3Fe(CN)6 

K4Fe(CN)6 

0.4687 
0.9628 
1.949 

309 
275.3 
200.8 

66.64 
55.19 
35.95 

(Grube.) 
Solubility  in  KOH+Aq  at  25°. 


KOH  Normality 


0.4687 
0.9628 
1.949 


g.  K3Fe(CN)6  per  1. 


342.7 
302.3 
215.1 


(Grube,  Z.  Electrochem,  1914,  20.  342.) 

Insol.  in  liquid  NH3.     (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 


336 


FERRICYANIDE,  POTASSIUM  SODIUM 


Insol.  in  absolute  alcohol,  and  only  si.  sol. 
in  dil.  alcohol. 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

Insol.  in  methyl  acetate  (  Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,  43,  314.) 

Insol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1370.) 

Potassium    sodium    ferricyanide, 

KNa2Fe(CN)6. 
Sol.  in  H2O. 

K2NaFe(CN)6.    Sol.  in  H2O. 
K3Na3[Fe(CN)6]2.    Sol.  in  H2O. 
+3H2O. 

Potassium  ferricyanide  iodide,  K3Fe(CN)3, 

KI. 
Very  unstable. 

Silver  ferricyanide,  Ag3Fe(CN)6. 

1  1.  H2O  dissolves  0.00066  g.  Ag3Fe(CN)6 
at  20°.  (Whitby,  Z.  anorg.  1910,  67.  108.) 

Sol.  in  NH4OH,  and  hot  (NH4)2CO3+Aq, 
but  insol.  in  NH4  salts  +Aq. 

Insol.  in  Hg(NO3)2+Aq.  (Wackenroder, 
A.  41.  317.) 

Silver  ferricyanide  ammonia,  2Ag3Fe(CN)6, 


Insol.  in  H2O.  Sol.  in  NH4OH+Aq. 
(Gintl.) 

2Ag3Fe(CN)6,  5NH3.  (Carlo,  Gazz.  ch. 
it.  1910,  40.  (2)  477.) 

Sodium  ferricyanide,   Na3Fe(CN)6+H2O. 

Deliquescent.    Sol.  in  5.3  pts.  cold,  and  1.5 
pts.  boiling  H2O.    Insol.  in  alcohol,  but  not 
pptd.    thereby   from   aqueous   solution. 
(Bette.) 

Ferrinitrososulphydric  acid. 

See  Ferrofteptanitrososulphydric  acid. 

Ferrocyanhydric  acid,  H4Fe(CN)6. 

Sol.  in  H2O  and  alcohol. 

100  pts.  H2O  dissolve  15  pts.  acid  at  14°. 
(Joannis,  A.  ch.  (5)  26.  514.) 

Insol.  in  ether,  and  much  less  sol.  in  ether- 
alcohol  than  in  alcohol.  Insol.  in  cone. 
HCl+Aq. 

Ferrocyanides. 

The  ferrocyanides  of  the  alkali  and  alka- 
line-earth metals  are  sol.  in  H2O;  the  others 
are  insol.,  but  sol.  in  alkalies  +Aq  in  case  the 
base  is  sol.  therein. 

Aluminum  ferrocyanide,  Al4[Fe(CN)s]3  + 
17H2O. 

SI.  sol.  in  H20. 

SI.  sol.  in  HCl+Aq  with  partial  decomp. 
(Wyrouboff,  A.  ch.  (5)  8.  446.) 


Ammonium  ferrocyanide,   (NH4)4Fe(CN)6  + 

3H20. 

Very  sol.  in  H2O;  insol.  in  alcohol. 
+H2O.    (Berzelius.) 

Ammonium  cadmium  ferrocyanide  ammonia, 

(NH4)2Cd3[Fe(CN)6]2,  2NH3+H2O. 
Sol.  in  H2O.     (Wyrouboff,  A.  ch.  (5)  10. 
413.) 

Ammonium  calcium  ferrocyanide, 

(NH4)2CaFe(CN)6. 

SI.  sol.  in  H2O.  (Kunheim  and  Zimmer- 
man, Dingl.  252.  47'8.) 

100  g.  sat.  solution  in  H2O  contain  0.258 
g.  at  16°.  (Brown,  J.  phys.  Ch.  1898,  2.  51.) 

Ammonium  cuprous  ferro  cyanide, 

(NH4)2Cu2Fe(CN)6. 
Insol.  in  H2O  and  alcohol. 
Decomp.  in  the  air.     (Messner,  Z.  anorg. 
1895,  8.  382.) 

Ammonium   cu 


ionium   cupric   ferrocyanide, 

(NH4)2CuFe(CN)6. 


Ppt. 

+xH2O.  Very  unstable.  Insol.  in  H2O; 
decomp.  by  boiling  H2O.  (Messner,  Z.  anorg. 
1895,  8.  384.) 

Ammonium  lithium  ferrocyanide, 

(NH4)2Li2Fe(CN)6+3H2O. 
Sol.  in  H2O.     (Wyrouboff,  A.  ch.  (4)  21. 
270.) 

Ammonium  magnesium  ferrocyanide. 

(NH4)2MgFe(CN)6. 

1  1.  sat.  solution  at  17°  contains  2.48  g. 
(NH4)2MgFe(CN)«.  (Robinson,  Chem.  Soc. 
1909,  95.  1353.) 

Ammonium  manganous  ferrocyanide, 

(NH4)2MnFe(CN)6. 
Ppt.    (Blum,  Z.  anal.  30.  284.) 

Ammonium    potassium    ferrocyanide, 
NH4K3Fe(CN)6+3H20. 

Easily  sol.  in  cold,  more  easily  in  hot  H2O. 
Insol.  in  alcohol. 

(NH4)2K2Fe(CN)G+3H2O.     Sol.  in  H2O. 

Ammonium  potassium  ferrocyanide  ammo- 
nium   chloride,     (NH4)3KFe(CN)6, 
2NH4C1. 
Sol.  in  H2O.    (Etard,  J.  pr.  (2)  31.  430.) 

Ammonium  ferrocyanide   bromide, 

(NH4)4Fe(CN)6,  2NH4Br. 
Permanent.    Very  sol.  in  H2O. 

Ammonium    ferrocyanide    chloride, 

(NH4)4Fe(CN)6,  2NH4C1+3H20. 
Permanent.    Very  sol.  in  H2O,  but  less  so 
than    NH4C1.      (Bunsen.) 


FERROCYANIDE,  CUPROUS 


337 


Antimony    ferrocyanide, 

25H2O. 
Ppt.    (Atterberg.) 


Sb4[Fe(CN)6]3  + 


Barium  ferrocyanide,  Ba2Fe(CN)6+6H2O. 

Permanent.    SI.  sol.  in  H2O. 

Sol.  in  584  pts.  cold,  and  116  pts.  boiling 
H2O  (Duflos,  1832);  sol.  in  1800  pts.  cold 
H2O  (Porrett,  1814);  sol.  in  1920  pts.  cold, 
and  about  100  pts.  boiling  H2O  (Thomson); 
sol.  in  2000  pts.  cold,  and  100  pts.  boiling 
H2O.  (Ure'sDict.) 

Sol.  in  1000  pts.  H2O  at  15°,  and  100  pts.  at 
75°.  (Wyrouboff,  A.  ch.  (4)  16.  292.) 

Sol.  in  HNO3,  HC1,  or  cone.  H2SO4+Aq. 

Barium  cupric  ferrocyanide,  BaCuFe(CN)6. 

Insol.  in  H2O.  (Messner,  Z.  anorg.  1895, 
8.  389.) 

Barium  potassium  ferrocyanide, 
BaK2Fe(CN)6+3H2O. 

Sol.  in  38  pts.  cold,  and  9.5  pts.  boiling  H2O 
(Duflos,  1832);  in  36.4  pts.  H20  at  14°,  and 
11.9  pts.  at  b.-pt.  (Mosander.) 

Not  more  sol.  in  NH4Cl+Aq  than  in  H2O. 
Sol.  in  dil.,  insol.  in  cone.  HCl+Aq.  (Rose.) 

+5H2O.  Sol.  in  300  pts.  H2O  at  ord.  temp. 
(Wyrouboff.) 


Bismuth  ferrocyanide, 
5H20(?). 

SI.  sol.  in  pure  H2O. 

Bi4[Fe(CN)6]5.  Ppt. 
31.  657.) 


Bi2Fe(CN)6  + 

(Wyrouboff.) 
(Muir,  Chem.  Soc. 


Bismuth  potassium  ferrocyanide, 

BiKFe(CN)6+7H2O,  or  4H2O. 
Ppt. 

Cadmium  potassium  ferrocyanide, 

CdK2Fe(CN)6+H2O. 
Insol.  in  H20. 
Formula  given  by  Wyrouboff  is 

Cd5K6lFe(CN)6]4  + 1 1H20  (?) . 

Calcium  ferrocyanide,  Ca2Fe(CN)6+12H2O. 
Very  sol.  in  H2O.  Sol.  in  0.66  pt.  H20  at 
90°  and  not  pptd.  by  cooling,  and  is  ap- 
parently less  sol.  in  warm  than  cold  H2O. 
(Wyrouboff,  A.  ch.  (4)  16.  280.) 

Calcium  cuprous  ferrocyanide, 

CaCu2Fe(CN)6.      (Messner,     Z.    anorg. 
1894,  8.  387.) 

Calcium  cupric  ferrocyanide,  CaCuFe(CN)6. 

Insol.  in  H2O.      (Messner,  Z.  anorg.  1895 
8.  388.) 

Calcium  potassium  ferrocyanide, 

CaKjFe(CN).; 

SI.  sol.  in  H2O.     (Kunheim  and  Zimmer- 
man,  Dingl.   262.   478.) 


+3H2O.  Sol.  in  795  pts.  H2O  at  15°,  and 
145  pts.  at  b-pt.,  with  decomp.  in  the  latter 
case. 

Sol.  in  dil.,  insol.  in  cone.  HCl+Aq.  Sol. 
in  HNO3  of  1.2  sp.  gr.  (Mosander.) 

Insol.  in  NH4Cl+Aq. 

Calcium  sodium  ferrocyanide, 

CaNa6[Fe(CN)6]2. 
Sol.  in  H2O. 

Calcium  strontium  ferrocyanide, 

CaSrFe(CN)6  +  10H2O. 
Efflorescent.     Sol.  in  about  3  pts.  H20. 
(Wyrouboff,  A.  ch.  (4)  21.  278.) 

Cerium    ferrocyanide,    Ce4[Fe(CN)6]s+ 

30H20. 
Ppt.    (Wyrouboff.) 

Cerium   potassium   ferrocyanide, 

CeKFe(CN)6+3H20. 
Ppt.     (John.) 
+4H2O.     (Wyrouboff.) 


Chromic     ferrocyanide, 

20H2O. 
Ppt. 


Cr2[Fe(CN)6]3  + 


Cobaltous    ferrocyanide,    Co2Fe(CN)6  + 
7H20. 

Wholly  insol.  in  H2O. 

Sol.  in  H2SO4  with  decomp.  Insol.  in 
HCl+Aq.  SI.  sol.  in  NH4OH+Aq.  Sol.  in 
(NH4)2CO3+Aq.  Insol.  in  NH4Cl+Aq.  Sol. 
inKCN+Aq. 

Cobaltous  ferrocyanide  ammonia, 
Co2Fe(CN)6,  8NH3  +  10H2O. 

Ppt.  Decomp.  on  standing.  (Curda,  Z. 
Ch.  1869.  369.) 

Co2Fe(CN)6,  12NH3+9H2O.  As  above. 
(Curda.) 

Cobaltous  potassium  ferrocyanide, 

CoK2Fe(CN)6. 

Ppt.     (Wyrouboff.) 

Co5K5[Fe(CN)6]4  (?).  Ppt.  Insol.  onlyrin 
presence  of  an  excess  of  K4Fe(CN)6.  (Wy- 
rouboff.) 

Columbium    potassium    ferrocyanide, 

Cb16K[Fe(CN)6]2+67H2O  (?). 

Sol.  inH2O.    (Wyrouboff.) 

Cb12K2Fe(CN)6  +  39H2O  (?).  Sol.  in 
H20.  (W,.) 

(CbO)5K9[Fe(CN)6]6+10H20(?).  Ppt.  (At- 
terberg.) 

Cuprous  ferrocyanide,  Cu4Fe(CN)6. 

Insol.  in  H2O;  sol.  in  NH4OH+Aq;  insol. 
in  NH4Cl+Aq. 


338 


FERROCYANIDE,  CUPRIC,  BASIC 


Cupric  ferrocyanide,  basic,  CuFe(OH)4(CN)4. 
Ppt.  (Bong,  Bull.  Soc.  23. 231.) 

Cupric  ferrocyanide,  Cu2Fe(CN)6+7H2O. 

Insol.  in  H2O  or  acids.  -  Insol.  in  NH4 
salts +Aq.  Sol.  in  NH4OH+Aq.  Sol.  in 
(NH4)2C2O4+Aq  and  in  KCN+Aq. 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20. 827.) 

+  10H2O.  Sol.  in  excess  of  K4Fe(CN)6  + 
Aq,  especially  if  hot.  (Wyrouboff.) 

Cupric    ferrocyanide    ammonia    (cupram- 
monium     ferrocyanide),     Cu2Fe(CN)6, 
4NH3+H2O. 

Insol.  in  H2O  or  alcohol.  Sol.  in  NH4OH  + 
Aq.  (Bunsen.) 

Cu2Fe(CN)6,  8NH3+H20. 

Cuprous  magnesium  ferrocyanide, 

Cu2MgFe(CN)6. 

Very  unstable.     Decomp.  in  air. 
Insol.  in  H2O.     (Messner,  Z.  anorg.  1895, 
8.  385.) 

Cupric  magnesium  ferrocyanide, 

CuMgFe(CN)6. 

Insol.  in  H2O.  Decomp.  by  boiling  H2O. 
Very  unstable.  (Messner,  Z.  anorg.  1895,  8. 
387.) 

Cuprous  potassium  ferrocyanide, 

Cu2K2Fe(CN)6. 

Insol.  in  H2O.  Decomp.  by  boiling  H2O. 
Decomp.  by  acids.  Insol.  in  alcohol.  (Mess- 
ner, Z.  anorg.  1895,  8.  378.) 

+l>£HtO.  Insol.  in  H2O,  alcohol,  or  ether. 
Decomp.  by  acids.  Sol.  in  KCN+Aq. 

K3Cu2Fe(CN)6+4H2O. 

+5H2O.     (Wonfor.) 

+6H2O.     (Wyrouboff.) 

Cupric  potassium  ferrocyanide,  K2CuFe(CN)6 

+H20. 

Insol.  in  cold,  si.  decomp.  by  boiling  H2O. 
K2Cu,[Fe(CN)6]2  +  12H2O.    Ppt. 

Cuprous  sodium  ferrocyanide, 

Cu2Na2Fe(CN)6. 

Decomp.  by  boiling  H2O;  insol.  in  alcohol; 
insol.  in  H2O;  decomp.  by  acids.  (Messner, 
Z.  anorg.  1895,  8.  373.) 

Cupric    sodium   ferrocyanide, 

CuNa2Fe(CN)6. 

Insol.  in  cold  H2O.  Decomp.  by  boiling 
H2O.  (Moissan,  Z.  anorg.  1895,  8.  376.) 

Cupric     strontium    ferrocyanide, 

CuSrFe(CN)6. 

Insol.  in  H2O.  (Messner,  Z.  anorg.  1895, 
8.  389.) 


Didymium  potassium  ferrocyanide,. 
DiKFe(CN)6+4H2O. 

Ppt.    (Cleve.) 
+2H2O.    (Wyrouboff.) 

Erbium  potassium  ferrocyanide,  ErKFe(CN)6 

+zH2O. 
(Hoglund.) 

Gallium  ferrocyanide. 

Sol.  in  boiling  HCl+Aq.    (de  Boisbaudran, 
C.  R.  99.526.) 

Glucinum  ferrocyanide,  Gl2Fe(CN)6,  4G102H2 

+7H20  (?). 
Sol.  in  H2O.    (Atterberg.) 

Iron    (ferric)    ferrocyanide,    Fe7(CN)j8  = 

Fe4[Fe(CN)6]3+zH20. 
(Prussian  blue.)  Insol.  in  H2O,  alcohol, 
ether,  or  oils.  Decomp.  slowly  by  boiling 
H2O.  Insol.  in  dil.  mineral  acids.  Sol.  in 
cone.  HCl+Aq,  and  cone.  H2SO4  without  de- 
comp. Sol.  in  H2C204  or  NH4  tartrate+Aq. 
Insol.  in  NH4OH+Aq.  Decomp.  by  NaOH, 
or  KOH+Aq.  Not  pptd.  in  presence  of  tar- 
trates  or  citrates. 

Iron   (ferrous)   potassium  ferrocyanide, 

FeK2Fe(CN)6. 
Insol.  in  H2O.    Decomp.  on  air. 

Iron    (ferric)    potassium    ferrocyanide, 

FeKFe(CN)6. 

Is  probably  ferrous  potassium  ferricyanide, 
which  see. 

Iron    (ferric)    ferrocyanide   ammonia, 

Fe4[Fe(CN)6]3,  6NH3+9H2O. 
Insol.  in  NH4  tartrate+Aq. 

Lanthanum  potassium  ferrocyanide, 

LaKFe(CN)6+4H2O. 
Ppt. 

Lead  ferrocyanide,  Pb2Fe(CN)6+3H2O. 

Insol.    in    H2O,    acids,    or    NH4OH+Aq. 
(Wyrouboff,  A.  ch.  (5)  8.  480.) 

SI.  sol.  in  cone.  H2SO4,  from  which  it  is 
pptd.  by  H2O.    (Berzelius.) 

Sol.  in  hot  NH4C1,  or  NH4  succinate+Aq; 
insol.  in  other  NH4  salts +Aq.     (Wittstein.) 

Insol.  in  NH4Cl+Aq.     (Brett.) 

Not  pptd.  in  presence  of  Na  citrate. 
(Spiller.) 

Lithium  ferrocyanide,  Li4Fe(CN)6+9H2O. 
Deliquescent.    Very  sol.  in  H2O. 

Lithium  potassium  ferrocyanide, 

Li2K2Fe(CN)6+3H2O. 
Very  sol.  in  H2O.    Sol.  in  1.5  pts.  H2O  at 
ord.  temp.    (Wyrouboff,  A.  ch.  (4)  21.  274.) 


FERROCYANIDE,  POTASSIUM 


339 


Magnesium    ferrocyanide,    Mg2Fe(CN)6+ 
6H2O. 

Sol.  in  3  pts.  cold  H2O.     (Bette,  A    22 

148.) 

Magnesium  potassium  ferrocyanide. 
MgK,Fe(CN).. 

Sol.  in  1575  pts.  H2O  at  15°,  and  238  pts.  at 
100°.     Solution  is  decomp.   by  boiling 
(Storer's  Diet.) 

1  1.  sat.  solution  at  17°  contains  1.95  g 
MgK2Fe(CN)6.  (Robinson,  Chem.  Soc 
1909,  75.  1353.) 

Manganous    ferrocyanide,    Mn2Fe(CN)6+ 
7H2O. 

Insol.  in  H20.  Sol.  in  HCl+Aq.  Insol  in 
NH4C1,  or  NH4NO3+Aq. 

Manganic  ferrocyanide,  Mn2Fe3(CN)i2. 

Insol.  in  H2O.  Easily  decomp.  in  the  air 
Sol.  in  HC1.  (Straus,  Z.  anorg.  1895,  9.  8.) 

Manganous  potassium  ferrocyanide, 

MnK2Fe(CN)6. 
Ppt.     (Berzelius.) 

5Mn2Fe(CN>,   4K4Fe(CN)6+4H2O(?). 
Ppt.    Sol.  in  dil.  HCl+Aq.    (Wyrouboff.) 

Mercuric    potassium    ferrocyanide. 

K2HgFe(CN)6. 

Insol.  in  H2O.  Appreciably  sol.  in 
K4Fe(CN)6+Aq.  (Fernekes,  J.  Am.  Chem. 
Soc.  1906,  28.  87.) 

Molybdenum  ferrocyanide,  Mo4Fe(CN)6+ 
20H2O(?).  . 

Very  sol.  in  NH4OH+Aq.     (Wyrouboff.) 

Mo2Fe(CN)6+8H2O  (?).     (W.) 
+  14H2O  (?).    Very  sol.  in  H2O;  insol  .in 
alcohol.    (W.) 

Molybdenum  potassium  ferrocyanide. 

K4Mo8[Fe(CN)6]2+40H20  (?). 

(Wyrouboff.) 

K2(Mo02)3[Fe(CN)6j2,  2MoO3+20H2O  (?). 
(Atterberg.) 

K6Mo2[Fe(CN)6]2,    2MoO3  +  12H2O    (?). 
(Atterberg.) 

Nickel  ferrocyanide,  Ni2Fe(CN)6+llH2O,  or 
14H2O. 

Ppt.  Insol.  in  H2O  or  HCl+Aq.  Sol.  in 
NH4OH+Aq;  insol.  in  NH4  salts +Aq.  Sol. 
in  KCN+Aq. 

Nickel  ferrocyanide  ammonia,  Ni2Fe(CN)6, 
4NH3+H2O. 

Completely  insol.  in  H2O  and  not  attacked 
thereby;  sol.  in  NH4OH+Aq  to  form— 

Ni2Fe(CN)6,  10NH3+4H2O.  Decomp.  by 
hot  H2O.  (Reynoso,  A.  ch.  (3)  30.  252.) 

Ni2Fe(CN)6,  2NH3+4,  and  9H2O.    Hygro- 


scopic.   Easily  decomp.    (Gintl,  J.  B.  1868. 

Ni2Fe(CN)6,  8NH3+4H2O.  Sol.  in 
NH4OH+Aq.  (G.) 

Ni2Fe(CN)6,  12NH3+9H20.  Sol.  in 
NH4OH+Aq,  but  less  so  than  the  above 
compounds.  (G.) 

Nickel  potassium  ferrocyanide,  NiK2Fe(CN)6 
+3H2O. 

Ppt.     (Wyrouboff.) 
Osmium  ferrocyanide,  Os2Fe(CN)6. 

Ppt.    (Martius,  A.  117.  368.) 
Potassium  ferrocyanide,  K4Fe(CN)6. 

Permanent.  Easily  sol.  in  cold,  and  more 
easily  in  hot  H2O. 

Sol.  in  4.23  pts.  H2O  at  15°,  or  100  pts."H2O 
dissolve  23.6  pts.  salt  at  15°.  (Schiff,  A.  113. 
350.) 

100  pts.  H20  dissolve  27.8  pts.  at  12.2°; 
65.8  pts.  at  37.7°;  87.6  pts.  at  65.5°:  and  90.6 
pts.  at  96.3°.  (Thomson.) 

Sol.  in  4  pts.  cold,  and  2  pts.  boiling  H2O. 
(Wittstein.) 

100  pts.  H20  dissolve  29.2  pts.  salt  at  15°, 
and  solution  has  sp.  gr.  =  1.1441.  (Michel 
and  Kraft,  A.  ch.  (3)  41.  478.) 

Solubility  of  K4Fe(CN)6  in  H2O  at  t°. 
—2°       +7°       14°         30°         56° 
10.8    '15.4      17.9      23.0      31.7% 
60°        75°        89°         98°         157° 
34.0      39.1      41.9      42.6      46.8% 
(Etard,  A.  ch.  1894,  (7)  2.  546.) 

K4Fe(CN)6+Aq  sat.  at  8°  has  sp.  gr.= 
1.13.  (Anthon.) 

Sp.  gr.  of  K4Fe(CN)6+Aq  at  15°. 


OB 
|1 

1"! 
g 

Sp.  gr. 

§ 

o 

11 

^ 

Sp.  gr. 

"O^- 

11 

£S 

Sp.  gr. 

i 

2 
3 
4 
5 
6 
7 

1.0058 
1.0116 
1.0175 
1.0234 
1.0295 
1  .  0356 
1.0417 

8 
9 
10 
11 
12 
13 
14 

1.0479 
1.0542 
1  .  0605 
1.0669 
1.0734 
1.0800 
1.0866 

15 
16 
17 
18 
19 
20 

1.0932 
1.0999 
1.1067 
1.1136 
1  .  1205 
1  .  1275 

(Schiff,  A.  113.  199.) 
Sp.  gr.  of  K4Fe(CN),+Aq  at  25°. 

Concentration  of 

K4Fe(CN)6+Aq. 

Sp.  gr. 

1  —  normal 
]A—     " 

'A—    " 

Vs—      " 

Vl6—         " 

1.0617 
1.0300 
1.0150 
1.0074 
1.0037 

(Wagner,  Z.  phys.  Ch.  1890,  6.  37.) 

340 


FERROCYANIDE,  POTASSIUM  SAMARIUM 


Solubility  in  KOH+Aq  at  25°. 


KOH  Normality 

g.  K4Fe(CN)6+3H2Operl. 

0.09984 

0.2496 
0.4963 
0.7036 
0.9415 
1.395 
1.883 

308.5 
283.5 
247.1 
217.4 
184.8 
132.1 
86.12 

(Grube,  Z.  Electrochem,  1914,  20.  342.) 

K4Fe(CN)6+NaCl+Aq  sat.  at  20°  con- 
tains 26.6  g.  NaCl  and  17.8  g.  K4Fe(CN)6 
per  100  g.  H2O;  sat,  at  93°  it  contains  27.4  g. 
NaCl  and  35.9  g.  K4Fe(CN)6  per  100  g.  H2O. 
(Cohroy,  J.  Soc.  Chem.  Ind.  1898,  17.  105.) 

K4Fe(CN)6+KCl+Aq  sat.  at  21°  con- 
tains 27.2  g.  KC1  and  4.2  g.  K4Fe(CN)6  per 
100  g.  H2O;  sat.  at  99°  it  contains  39.6  g. 
KC1  and  17.0  g.  K4Fe(CN)6  per  100  g.  H2O. 
(Conroy.) 

K4Fe(CN)6+Na2CO3+Aq.     sat.     at    22° 
contains  29.9   g.   Na2CO3   and  26.7   g. 
K4Fe(CN)6  per  100  g.  H20;  sat.  at  97°  it  con- 
tains 42.0  g.  Na2CO3  and  27.5  g.  K4Fe(CN)6 
per  100  g.  H2O.    (Conroy.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Insol.  in  alcohol  even  when  dilute. 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1904,  37.  3601.) 

Insol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1370.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

+3H2O.  1  1.  sat.  salution  in  H2O  contains 
319.4  g.  K4Fe(CN)6+3H2O.  (Grube,  Elec- 
trochem, Z.  1914,  20.  342.) 

Two  modifications  with  different  solubil- 
ities. 

25.0  g.  of  a  modification  are  contained  in 
100  g.  of  salution  at  20°. 

24.6  g.  of  £  modification  are  contained  in 
100  g.  of  solution  at  20°.  (Briggs,  Chem. 
Soc.  1911,  99.  1024.) 

32.0  g.  K4Fe(CN)6  (anhydrous)  are  dis- 
solved in  100  g.  H2O  at  25°.  (Wagner,  Z. 
phys.  Ch.  1910,  71.  428.) 

Potassium  samarium  ferrocyanide, 

KSmFe(CN)6+5H2O. 
Precipitate.    (Cleve.) 

Potassium  sodium  ferrocyanide, 

KNa3Fe(CN)6+12H2O. 

Sol.  in  H2O. 

K2Na2Fe(CN)6+8H2O.   Easily  sol.  in  H2O. 
K3NaFe(CN)6+3H2O.     Permanent.     Eas- 
ily sol.  in  H2O;  insol.  in  alcohol. 

Potassium    sodium    ferrocyanide    nitrate, 

K2Na2Fe(CN)6,  4KNO3. 
Sol.  inH2O.    (Martius.) 


Potassium  strontium  ferrocyanide, 

K2SrFe(CN)6+3H20. 
Easily  decomp.     Sol.  in  H2O;'sl.  sol.  in 
alcohol.    (Wyrouboff,  A.  ch.  (4)  21.  276..) 


Potassium  stannic  ferrocyanide, 

KSn3[Fe(CN)6]3+68H2O  (?) 

Ppt.    (Wyrouboff.) 

K4Sn10[Fe(CN)6]u+230H20    ( 
berg.) 


(Atter- 


Potassium  titanium  ferrocyanide, 

K3Ti3[Fe(CN)6]2  +  llH20  (?). 

Ppt.  Sol.  in  K4Fe(CN)6+Aq.  (Wyrou- 
boff.) 

K4Fe(CN)6,  HTi2Fe(CN)6+43H2O  (?). 
Ppt.  (Wyrouboff.) 

K2(TiO)3[Fe(CN)6j2+23H2O  (?).  Ppt. 
(Atterberg.) 

K2(TiO)n[Fe(CN)6]6  +  HOH20  (?).  Ppt. 
(Atterberg.) 

Potassium  tungsten  ferrocyanide, 

KW2Fe(CN)6+7H2O  (?). 
Sol.  in  H2O.    (Wyrouboff.) 
K2W5Fe(CN)6+2bH2O  (?).     Sol.  in  H2O. 
(W.) 

Potassium  uranium  ferrocyanide, 

K2U3[Fe(CN)6]2+6H20  r?). 

Ppt.     (Wyrouboff.) 

K2(U02)3[Fe(CN)6]2+6H2O.  Ppt.  (Atter- 
berg.) -  * 

K6(U02)5[Fe(CN)6]4+12H20.  Sol.  inf_H2O. 
(Atterberg.) 

Potassium  vanadium  ferrocyanide, 

K18V[Fe(CN)6]6+39H2O  (?). 
Ppt.    SI.  sol.  in  H,O.    (Wyrouboff.) 
K6(VO)5[Fe(CN)6]4+60H2O(?).  Ppt.    (At- 
terberg.) 

Potassium  ytterbium  ferrocyanide, 

KYbFe(CN)6+3H20. 
Ppt.      Sol.    in    excess    K4Fe(CN)6+Aq. 
(Cleve,  Z.  anorg.  1902,  32.  140.) 

Potassium  yttrium  ferrocyanide, 

KYFe(CN)e+2H2O. 
Ppt.    (Wyrouboff,  A.  ch.  (5)  8.  444.) 

Potassium  zinc  ferrocyanide, 

K4Zn6[Fe(CN)e]4  +  12H2O. 
Absolutely  insol.  in  H2O.    (Wyrouboff,  A. 
ch.  (5)  8.  485.) 

Potassium  ferrocyanide  carbonyl, 

K8Fe(CN)6(CO)  +3^H2O. 
See  Carbonyl  ferrocyanide,  potassium. 

Rubidium  ferrocyanide,  Rb4Fe(CN)6+2H2O. 
Sol.  in  less  than  1  pt.  H2O  at  ord.  temp, 
with  great  absorption  of  heat.     (Wyrouboff. 
A.  ch.  (4)  16.  307. 


FERRONITROSULPHIDE,  POTASSIUM 


341 


Silver  ferrocyanide,  Ag4Fe(CN)6+H2O. 

Insol.  in  HoO  or  dil.  acids.  Insol.  in 
NH4OH,  or  NH4  salts  +  Aq.  Sol.  in  KCN 
+  Aq. 

Decomp.  by  warm  NH4OH+A-.  (Weith, 
Z.  Ch.  (2)  5.  381.) 

Silver  ferrocyanide  ammonia, 

Ag4Fe(CN)6,  2NH3+H20. 

(Wyrouboff.) 

+  6H2O.     (Gintl.) 

Sodium  ferrocyanide,  Na4Fe(CN)6+12H2O. 

Efflorescent.  Less  sol.  in  H2O  than 
K4Fe(CN)6.  Sol.  in  4.5  pts.  H2O  at  12°. 
(John.) 

100  pts.  H2O  at  15.5°  dissolve  22  pts. 
(Ure's  Diet.) 

100  pts.  H2O  dissolve  at: 
18°       20°  42°       53° 

16.7     17.875     30.2    37.1  pts.     Na4FeCN6, 
58°       60°          77°       80° 
41.7     42.5        54.8     59.2  pts.     Na4FeCN6, 

96°         98°         98.5° 

62.1       61.6    *  6. 30  pts.  Na4FeCN6. 
(Conroy,  J.  Soc.  Chem.  Ind.  1898;  17.  104.) 

+  10H2O. 

100  pts.  H2O  dissolve  at: 

18°       20°       42° 

29.45  31.85   58.5  pts.  Na4Fe(CN)6  +  10H2O, 

53°      58°       60° 

75.9    88.4     90. 2  pts.  Na4Fe(CN)6  +  10H2O, 

77°      80°      96° 

129.5  146.0157.0  pts.  Na4Fe(CN)6  +  10H20, 

98°  98.5° 

156.5        161 .0  pts.  Na4Fe(CN)6  +  10H2O. 

(Conroy.) 

Strontium  ferrocyanide,  Sr2Fe(CN)6+15H2O. 

Efflorescent.  Sol.  in  2  pts.  cold,  and  less 
than  1  pt.  boiling  H2O.  (Bette.) 

Excessively  sol.  in  H2O.  (Wyrouboff,  A. 
ch.  (4)  16.  280.) 

+8H2O.     (Wyrouboff.) 

Thallous  ferrocyanide,  Tl4Fe(CN)6+2H2O. 

100  pts.  H2O  dissolve  0.37  pt.  at  18°,  and 
3.93  pts.  at  101°.  (Lamy.) 

Sol.  in  KCN+Aq.    (Kuhlmann.) 

Thorium  ferrocyanide,  ThFe(CN)6+4H2O. 
Ppt.    (Cleve,  Bull.  Soc.  (2)  24.  355.) 

Tin  (stannous)  ferrocyanide,  Sn2Fe(CN)6  + 

4H2O. 

Insol.  in  H2O  or  acids;  si.  sol.  in  NH4OH  + 
Aq.  (Wyrouboff.) 

Tin  (stannic)  ferrocyanide,  Sn5[Fe(CN)6]2  + 

18^H2O  (?). 
(Wyrouboff.) 


Titanium  ferrocyanide,  Ti7[Fe(CN)6]2  (?). 
Ppt.     (Wyrouboff.) 

Uranium  ferrocyanide,  UFe(CN)6  +  10H2O. 
Ppt.     (Wyrouboff.) 

Vanadyl  ferrocyanide,   (VO)2Fe(CN)6+ 

11H2O. 
Ppt.    (Atterberg.) 

Yttrium  ferrocyanide,  Y4[Fe(CN)6]3. 

Easily  sol.  in  H2O;  insol.  in  alcohol.  (Popp, 
A.  131.  179.) 

Zinc  ferrocyanide,  Zn2Fe(CN)6+3H2O. 

Insol.  in  H2O  or  acids. 

Insol.  in  HCl+Aq.  (Lea,  Sill.  Am.  J.  (2) 
31.  191.) 

Sol.  in  NH4OH,  or  NH4  salts+Aq.  (Witt- 
stein.) 

Insol.  in  NH4C1,  or  NH4NO+Aq.    (Brett.) 

SI.  sol.  in  boiling  K4Fe(CN)6,  or  K3Fe(CN)6 
+Aq.  (Gore.) 

Na4Fe(CN)6+NaCl+Aq  sat.  at  21°  con- 
tains 29.0  g.  NaCl  and  5.8  g.  Na4Fe(CN)6  per 
100  g.  H2O;  sat,  at  90°  it  contains  24.7  g. 
NaCl  and  21.3  g.  Na4Fe(CN)6  per  100  g.  H2O. 
(Conroy,  J.  Soc.  Chem.  Ind.  1898,  17.  105.) 

Na4Fe(CN)6+Na2CO3+Aq    sat.     at    22° 
contains     22.6     g.     Na2CO3     and     6.5     g. 
Na4Fe(CN)6  per  100  g.  H2O;  sat.  at  95°  it 
contains  29.8  g.   Na2CO3   and   36.8   g. 
Na4Fe(CN)6  per  100  g.  H2O.    (Conroy.) 

Very  si.  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  830.) 

Insol.  in  alcohol. 

+4H2O.  Absolutely  insol.  in  H2O. 
(Wyrouboff,  A.  ch.  (5)  8.  485.) 

+8H2O.     (Weith,  A.  147.  329.) 

+  10H2O.     (Pebal,  A.  233.  165.) 

Ferro^ranitrososulphydric  acid, 

H2S2(NO)4Fe2. 

Insol.  in  H2O;  si.  sol.  in  alcohol;  more 
easily  in  ether;  very  sol.  in  CS2  or  CHC13. 
Not  obtained  in  a  pure  state.  (Pawel,  B. 
16.  2600.) 

Ethyl  ferro^ranitrososulphide, 

(C2H5)S2(NO)4Fe2. 

Insol.  in  H2O,  difficultly  sol.  in  alcohol, 
more  easily  in  ether,  and  very  easily  in  CS2, 
CHC1,,  C2H5I,  or  C6H6.  (Pawel,  B.  16. 
2609.) 

Ferrous ,  FeS2(NO)4Fe2. 

More  difficultly  sol.  in  H2O  and  alcohol 
than  the  hepta  salt. 

Sol.  in  ether. 

Potassium ,  K2S2(NO)4Fe2+4H2O. 

Sol.  in  H2O.  Easily  sol.  in  alcohol;  insol. 
in  ether.  (Pawel,  B.  16.  2600.) 

True    composition    of    "  nitrosulphide    of 


342 


FERRONITROSOSULPHIDE,  SODIUM 


iron  and  potassium"  of  Roussin.     (A.  ch. 
(3)  52.  297.)     (Pawel,  B.  13.  1949.) 

Sodium  ferroteZranitrososulphide, 
Na2S2(NO)4Fe2+8H2O. 

Sol.  in  H2O;  easily  sol.  in  alcohol;  insol. 
in  ether.  (Pawel.) 

True  composition  of  "nitrosulphide  of 
iron  and  sodium"  of  Roussin.  (Pawel.) 

Thallium ,  Tl2S2(NO)4Fe2. 

Insol.  in  H2O,  alcohol,  or  ether.     (Pawel.) 

Ferro/iep/anitrososulphydric  acid. 
HS3(NO)7  Fe4. 

Insol.  in  H2O,  alcohol,  and  ether.  Easily 
sol.  in  CS2  or  CHC13.  (Pawel,  B.  15.  2604.) 

May  be  called  Ferrinitrososulphydric  acid. 

Ammonium  ferroAeptonitrososulphide, 
NH4S3(NO)7  Fe4+H2O. 

Less  easily  sol.  in  H20  than  the  K  com- 
pound. (Pawel,  B.  15.  2600.) 

"Binitrosulphide  of  iron"  of  Roussin.  Sol. 
in  about  2  pts.  boiling  H2O;  very  si.  sol.  in 
cold  H2O.  Very  sol.  in  alcohols,  methyl, 
ethyl,  or  amyl,  and  in  HC2H3O2.  Miscible 
with  ether.  Insol.  in  CS2  or  CHC13. 

Decomp.  by  cone.  HC1,  HNO3,  or  H2SO4. 

Not  attacked  by  H2C2O4,  or  H2C4H4O6  + 
Aq. 

Insol.  in  NH4OH,  and  KOH+Aq.  (Rous- 
sin, A.  ch.  (3)  52.  286.) 

Sol.  in  H2O.  Insol.  in  alcohol.  (Hofmann, 
Z.  anorg.  1895,  9.  299.) 

Barium . 

Easily  sol.  in  H2O.    (Pawel.) 

Caesium ,  Fe4(NO)7  S3Cs+H2O. 

Insol.  in  H2O.  Difficultly  sol.  in  alcohol 
and  ether.  (Pawel.) 

Sparingly  sol.  in  H2O.  (Hofmann,  Z. 
anorg.  1895,  9.  298.) 

Calcium . 

Easily  sol.  in  H2O.    (Pawel.) 

Ferrous ,  Fe[S3(NO)7  Fe4]2+8H2O. 

More  easily  so],  in  H2O  than  Na  salt. 
(Pawel.) 

Lead . 

Difficultly  sol.  in  H2O.    (Pawel.) 

Magnesium . 

Easily  sol.  in  H2O.    (Pawel.) 

Potassium — — ,  KS3(NO)7  Fe4. 

Sol.  in  H2O,  alcohol,  and  very  sol.  in  ether 
with  slight  decomp.  (Pawel,  B.  15.  2600.) 


Rubidium  feiroheptamtroso sulphide, 
RbS3(NO)7  Fe4. 

Less  soluble  in  H2O  than  the  NH4  salt. 
(Pawel.) 

+H2O.  Ppt.  (Hofmann,  Z.  anorg.  1895, 
9.298.) 

Sodium ,  NaS3(NO)7  Fe4+2H2O. 

More  sol.  in  H20  than  the  potassium  salt. 
(Pawel.) 

Thallium ,  T1S3(NO)7  Fe4+H2O. 

Very  difficultly  sol.  in  H20.  More  easily 
sol.  in  alcohol.  (Pawel.)  (Hofmann,  Z. 
anorg.  1895,  9.  297.) 

Ferrodinitrosothiosulphonic  acid. 

Ammonium  ferrodmitrosothiosulphonate, 

Fe(NO)2S203NH4+H20. 
Can  be  cryst.  from  warm  H2O  without  de- 
comp.   (Hofmann,  Z.  anorg.  1895,  8.  321.) 

Caesium ,  Fe(NO)2S2O3Cs. 

Sparingly  sol.  in  H2O.    (Hofmann.) 

Potassium ,  Fe(NO)2S2O3K+H2O. 

SI.  sol.  in  H2O  without  decomp.  atT80°. 

Sol.  in  50%  alcohol. 

Sol.  in  H2SO4  without  decomp.  (Hof- 
mann) . 

Rubidium ,  Fe(NO)2S2O3Rb+H20. 

Less  sol.  in  H2O  than  the  corresponding 
Na  salt.  (Hofmann.) 

Sodium ,  Fe(NO)2S2O3Na+2H2O. 

Closely  resembles  K  salt,  but  is  more  sol. 
in  H2O  and  alcohol.  (Hofmann.) 

Ferrotungstic  acid. 

Sol.  in  H2O.    (Laurent,  C.  R.  31.  693.) 

Ammonium  manganous  ferrotungstate. 
12(NH4)20,    6MnO,    2Fe203,    3H2O, 
45W03+81H20. 
Sol.  in  H2O.    (Laurent.) 

Barium    ferrotungstate,    21BaO,    2Fe2O3, 

45W03+27H20. 
Sol.  in  H2O.    (Laurent.) 

Potassium  ferrotungstate,  9K2O,  2Fe2O3, 
12H20,  45W03+54H20. 

Sol.  in  H2O.    (Laurent.) 

18K2O,  2Fe203,  3H2O,  45W03+54H2O. 
(Laurent.) 

Ferrous  acid. 

Barium  ferrite,  BaO,  Fe2O3. 
Ppt.    (List,  B.  11.  1512.) 


FLUOBORIDE,  CALCIUM 


343 


Calcium  ferrite,  4CaQ,  Fe2O3. 

Insol.  in  H2O,  or  sugar+H2O.  Decomp. 
by  the  weakest  acids,  but  not  by  boiling 
KOH+Aq.  (Pelouze,  A.  ch.  (3)  33.  5.) 

CaO,  Fe203.     (List.) 

3CaO,  Fe2O?.  Much  less  readily  attacked 
by  H2O  and  acids  than  the  silicates.  (Hilpert, 
B.  1909,  42.  4581.) 

3CaO,  2Fe2O3.  As  above.  (Hilpert,  B. 
1909,  42.  4581.) 

Calcium  ferrite  chloride,  CaO,  Fe2O3,  CaCl2. 
Not  decomp.  by  H20.    (Chatelier,  C.  R.  99. 
276.)     . 

Cupric  ferrite,  CuO,  Fe2O3. 
Ppt.    (List.) 
+5H2O.     (List.) 

arge 

Fe2O3  (?). 

Easily  decomp.  by  HCl+Aq.  Not  com- 
pletely sol.  in  dil.  HNO3+Aq.  Easily  sol.  in 
cone.  HN03.  Decomp.  by  acetic  acid. 
(Rose,  Pogg.  10.  323.) 

Magnesium  ferrite,  MgO,  Fe2O3. 

Insol.  in  H2O.  Not  attacked  by  boiling 
cone.  HNO3.  (Deville.  C.  R.  52.  1264.) 

Min.  Magnesioferrite.  Difficultly  sol.  in 
HCl+Aq.  (Rammelsberg,  Pogg.  107.  451.) 

+4H2O.    Ppt.    (List,  B.  11.  1512.) 

6MgO,  Fe2O3+9H2O.    Ppt. 

+15H2O.     Min.  Pyroaurite. 

i 

Manganous  ferrite,  MnO,  Fe2O3.          .ir«   \ 
Ppt.    (List.) 

Nickel  ferrite,  NiO,  Fe2O3. 
Ppt.    (List.) 

Potassium  ferrite,  3K2O,  4Fe2O3. 

Decomp.  by  H2O,  KOH+Aq,  NaOH+Aq, 
etc.,  but  only  slowly  by  NH4Cl+Aq.  (Salm- 
Horstmar,  J.  pr.  55.  349.) 

K2Fe2O4.  Decomp.  by  H2O.  (Rousseau 
and  Bernheim,  C.  R.  107. 240.) 

Silver  (argentous)  ferrite,  Ag4O,  Fe2O3  (?). 
Decomp.  by  dil.  HNO3+Aq.    (Rose,  Pogg. 
10.  323.) 

Sodium  ferrite,  Na2O,  Fe2O3. 

Na2O  is  dissolved  out  by  H2O.  Easily  sol. 
in  dil.  HCl+Aq.  Not  easily  decomp.  by 
NH4Cl+Aq.  (Salm-Horstmar.) 

Zinc  ferrite,  ZnO,  Fe2O3. 

Sol.  in  boiling  cone.  HCl+Aq.  (Ebel- 
men,  A.  ch.  (3)33.47.) 

Min.  Franklinite. 

Flavocobaltic  compounds. 

See  also  Xanthocobaltic  compounds. 


Flavocobaltic    chloraurate, 

(NO2)2Co(NH3)4AuCl4. 
More  easily  sol.    than  the  chloroplatinate. 
Not  wholly  insol.  in  absolute  alcohol.    (Jb'r- 
gensen,  Z.  anorg.  6.  159.) 

chloroplatinate,  [(NO2)2Co(NH3)4]2PtCl6 

As  the  chloroplatinite.    (Jorgensen.) 

chloroplatinite,  [(NO2)2Co(NH3)4]2PtCl4. 

Somewhat  sol.  in  H2O,  and  not  insol.  in 
50%  alcohol.  (Jorgensen.) 

chromate,  [(N02)2Co(NH3)4]2Cr207. 

Ppt.    (Jorgensen.) 

nitrate,  Co(NO2)2(NH3)4NO3. 

Sol.  in  about  33  pts.  cold  H2O;  insol.  in 
HNO3.  (Jorgensen.) 

Co(NO2)2(NH3)4NO3,  HNO3.  Decomp. 
by  H2O  or  alcohol.  (Jorgensen.) 

cobaltic  nitrite,  3(NO2)2Co(NH3)4, 

Co2(N02)6+2H20. 

SI.  sol.  in  H2O.  (Jorgensen,  Z.  anorg.  5. 
179.) 

diamine    cobaltic    nitrite, 

(N02)2Co(NH3)4, 
(N02)2(NH3)2Co(N02)2. 
Very  si.  sol.  in  H2O.    (Jorgensen.) 

sulphate,  [(N02)2Co(NH3)4]2S04. 

SI.  sol.  in  H2O,  more  easily  in  HC2H802  + 
Aq.  (Jorgensen.) 

Fluoborhydric  acid,  HBF4. 

Decomp.  by  H2O  very  rapidly.  (Landolph, 
C.  R.  86.  603.) 

Aluminum  fluoboride,  2A1F3,  3BF8. 

Sol.  in  H2O  only  when  acidulated;  sol.  in 
acids.  (Berzelius.) 

Ammonium  fluoboride,  NH4BF4. 

Easily  sol.  in  H2O.  Sol.  in  4  pts.  H2O  at 
16°,  and  1.02-1.05  pts.  boiling  H2O.  (Stolba, 
Chem.  techn.  Cent.  Anz.  7.  459.)  SI.  sol.  in 
alcohol. 

Barium  fluoboride,  Ba(BF4)2+2H2O. 

Deliquescent;  easily  sol.  in  H20;  decomp. 
by  alcohol.  (Berzelius.) 

Caesium  fluoboride,  CsBF4. 

100  pts.  H2O  dissolve  0.92  pt.  CsBF4  at  20°, 
and  0.04  pt.  at  100°.  (Godeffroy,  B.  9. 1367.) 

0.02  pts.  are  sol.  in  100  pts.  H2O  at  20°. 
(Erdmann,  Arch.  Pharm.  1894,  232.  21.) 

Calcium  fluoboride,  Ca(BF4)2. 

Decomp.  by  H2O,  with  formation  of  a  sol. 
acid  salt  and  an  insol.  basic  salt.  (Berzelius.) 


344 


FLUOBORIDE,  CUPBIC 


Cupric  fluoboride,  Cu(BF4)2. 

Deliquescent,  and  very  sol.  in  H2O.  (Ber- 
zelius.) 

Lead  fluoboride,  Pb(BF4)2. 

Sol.  in  H2O.  Decomp.  by  boiling  with 
H2O  or  alcohol  into  an  acid  soluble,  and  a 
basic  insoluble  salt.  (Berzelius.) 

Lithium  fluoboride,  LiBF4. 

Hygroscopic.  Easily  sol.  in  H2O.  (Ber- 
zelius.) 

Magnesium  fluoboride. 

Easily  sol.  in  H2O.     (Berzelius.) 

Potassium  fluoboride,  KBF4. 

Sol.  in  223  pts.  H2O  at  20°.    (Stolba.) 
Sol.  in  70.4  pts.  cold  H2O.    (Berzelius.) 
Sol.  in  15.94  pts.  H2O  at  100°.    (Stolba.) 
1.43  pts.  are  sol.  in  100  pts.  H2O  at  20°. 

(Erdmann,  Arch.  Pharm.  1894,  232.  21.) 
Not  more  sol.  in  NH4OH+Aq  than  in  H2O; 

sol',  in  hot  KOH,  NaOH,  or  M2CO3+Aq. 

(Berzelius.)       More    sol.     in     NH4Cl+Aq. 

(Rose,    Pogg.    80.    276.)      Insol.    in    20% 

KC2H3O2+Aq.       (Stromeyer.)       Insol.     in 

cold,  si.  sol.  in  boiling  alcohol. 

Rubidium  fluoboride,  RbBF4. 

100  pts.  H2O  dissolve  0.55  pt.  at  20°,  and 
1.0  pt.  at  100.°  (Godeffroy,  B.  9.  1337.) 

0.55  pts.  are  sol.  in  100  pts.  H2O  at  20°. 
(Erdmann,  Arch.  Pharm.  1894,  232.  21.) 

Sodium  fluoboride,  NaBF4. 

Easily  sol.  in  H20.  Very  si.  sol.  in  alcohol. 
(Berzelius.) 

Yttrium  fluoboride. 

Sol.  in  H2O  with  excess  of  acid.  (Berze- 
lius.) 

Zinc  fluoboride,  Zn(BF4)2. 

Deliquescent.    Sol.  in  H20.    (Berzelius.) 

Fluoboric  acid,  HBF4. 

See  Fluoborhydric  acid. 

H4B2O7,  3HF  and  H4B2O9,  2HF  (?).  Fume 
on  air,  and  are  decomp.  with  H2O.  (Lan- 
dolph,  B.  12.  1583.) 

HBO2,  3HF.  Decomp.  by  H2O.  (Ber- 
zelius, Pogg.  69.  644.) 

Is  either  a  mixture,  or  a  solution  of  HB02 
in  HF,  and  is  decomp.  by  distillation,  and  the 
salts  are  decomp.  by  recrystallisation.  (Bas- 
arow,  C.  R.  78. 1698.) 

Potassium  fluoborate,  K2B203F2  (?). 

SI.  deliquescent.  Scarcely  sol.  in  boiling 
alcohol.  (Schiff,  A.  Suppl.  6.  175.) 

See  Boron  fn'oxide  potassium  fluoride, 
B203,  2KF. 


Fluochromic  acid. 

Ammonium  fluochromate,  NH4CrO3F. 
Sol.  in  H20.     (Varenne,  C.  R.  91.  989.) 

Potassium  fluochromate,  KCrO3F. 

Efflorescent.  Sol.  in  H2O,  with  gradual 
decomp.  (Streng,  A.  129.  225.) 

Fluocolumbic  acid. 
See  also  Fluoxycolumbic  acid. 

Ammonium  fluocolumbate  fluoxycolumbate, 
(NH4)2CbF3,   2CbOF3,    NH4F. 

Cadmium    fluocolumbate,    Cd5H5Cb3F30  + 

28H20. 
Insol.  in,  and  decomp.  by  H2O.     (Streng.) 

Cobalt  fluocolumbate,  Co5H5Cb3F33+28H2O. 
Insol.  in,  and  decomp.  by  H2O.    (Streng.) 

Copper    fluocolumbate,    Cu2HCbFi0+9H2O. 
Insol.  in,  and  decomp.  by  H2O. 

Ferrous  fluocolumbate,  Fe3H4Cb2F20+19H2O. 
As  above. 

Manganous  fluocolumbate,   Mn5H5Cb3F3o+ 
28H2O. 

Mercuric  fluocolumbate,  Hg3CbFn+8H2O. 
As  above. 

Nickel  fluocolumbate,  Ni3H4Cb2F20+19H2O. 
As  above. 

Potassium  fluocolumbate,  K2CbF7. 

Decomp.  by  solution  in  H2O.  (Marignac 
A.  ch.  (4)  8.  34.) 

Rubidium  fluocolumbate,  Rb2CbF7. 

Sol.  in  H2O  and  HF+Aq.  Insol.  in  al- 
cohol. (Pennington,  J.  Am.  Chem.  Soc. 
1896,  18.  58.) 

Zinc  fluocolumbate,  Zn5H5Cb3F3o+28H20. 

Insol.  in  cold  H2O;  decomp.  by  hot  H80. 
(Santesson,  Bull.  Soc.  (2)  24.  52.) 

Fluodithionic  acid. 

Caesium  wonofluodithionate, 
S2O5(OH)FCs2+H2O. 

Easily  sol.  in  H2O  with  decomp. 

Sol.  in  HF;  very  unstable.  (Weinland,  Z. 
anorg.  1899,  21.  66.) 

Potassium  difluodithionate,  S2O5F2K2+3H2O. 
Easily  sol.  in  H2O  with  decomp. 
Sol.  in  HF;  very  unstable.    (Weinland.) 


FLUOPERBORATE,  POTASSIUM 


345 


Rubidium      cfcfluodithionate,      S2O5F2Rb2  + 

3H20. 

Easily  sol.  in  H2O  with  decomp. 
Sol.  in  HF;  very  unstable.    (Weinland.) 

Fluogermanic  acid,  H2GeF6. 

Known  only  in  solution.  (Winkler,  J.  pr. 
(2)  36.  177.) 

Potassium  fluogermanate,  K2GeF6. 

Sol.  in  173.98  pts.  H2O  at  18°.    (Winkler.) 
Sol.  in  184.61  pts.  H20  at  18°.    (Kriiss  and 

Nilson,  B.  20.  1696.) 

Sol.  in  34.07  pts.  H2O  at  100.°    (Winkler.) 
Sol.  in  38.76  pts.  H2O  at  100.°    (Kriiss  and 

Nilson.) 

Insol.  in  alcohol. 

IH'fluoiodic  acid. 

Ammonium  cfa'fluoiodate,  NH4IO2F2. 

Like  K  salt. 

Sol.  in  40%  HF+Aq.  (Weinland,  Z. 
anorg.  1899,  20.  30.) 

Sol.  in  H2O.  Easily  decomp.  (Weinland, 
B.  1897,30.868.) 

Caesium  cftfluoiodate,  CsIO2F2. 
(Weinland,  Z.  anorg.  1899,  20.  36.) 

Caesium    hydrogen    c&fluoiodate. 

CsI02F2,   HI02F2+2H20. 
Efflorescent.     Sol.  in  H2O  with  decomp. 
(Weinland,  Z.  anorg.  1899,  22.  257.) 

Potassium  dzfluoiodate,  KI02F2. 

Sol.  in  H20.  Decomp.  in  moist  air. 
(Weinland,  B.  1897,  30.  867. 

Decomp.  in  air.     Sol.  in  H2O  with  decomp. 
Sol.  without  decomp.  in  40%  HF+Aq. 
(Weinland,  Z.  anorg.  1899,  20.  31. 


Rubidium  cftfluoiodate,  RbIO2F2. 
Resembles    K    salt.      Sol.    in 
(Weinland,  Z.  anorg.  1899,  20.  35.) 


Rubidium  hydrogen  cfc'fluoiodate, 

RbIO2F2,HIO2F2  +2H2O. 
Sol.  in  40-60%  HF+Aq.     (Weinland,  Z. 
anorg.  1899,  22.  260.) 

Sodium  (ftfluoiodate,  NaIO2F2. 

Decomp.  by  H2O.    (Weinland,  B.  1897,  30. 
868.) 

Sol.  in  HF.    (Weinland,  Z.  anorg.  1899,  20. 

37.) 

Fluomanganic  acid,  H2MnF6. 

Decomp.  by  H2O.    Sol.  in  alcohol  and  ether 
in  absence  of  H2O.    (Nickles,  C.  R.  66.  107.) 


Ammonium  fluomanganate,  (NH4)2MnF6. 

More  sol.  than  the  K  salt.  (Nickles,  C.  R. 
65.  107.) 

True    composition    is    (NH4)4Mn2Fi0  = 
4NH4F,  Mn2F6.    (Christensen,  J.  pr.  (2)  34. 
41.) 

Cobalt   fluomanganate,    2CoF2,    Mn2F6  + 

8H2O. 
Sol.  in  H2O.    (Christensen.) 

Nickel     fluomanganate,     2NiF2,     Mn2F6  + 

8H2O. 
Sol.  in  H2O.     (Christensen.) 

Potassium  fluomanganate,  K2MnF6. 

Difficultly  sol.  in  H2O.  Decomp.  bv  much 
H2O.  (Nickles,  C.  R.  65.  107.) 

Composition  is  K4Mn2F10  =  4KF,  Mn2F6. 
Also  with  2H2O.  (Christensen,  J.  pr.  (2)  34. 
41.) 

Decomp.  by  H2O.  Sol.  in  HC1,  H2SO4  and 
HNO3  with  decomp.  Can  be  recryst.  from 
40%  HF+Aq.  Insol.  in  acetic  acid.  (Wein- 
land and  Lauenstein,  Z.  anorg.  1899,  20.  41.) 

Rubidium  fluomanganate,  Rb2MnF6+2H2O. 
As  the  K  salt.    (Weinland  and  Lauenstein. 
Z.  anorg.  1899,  20.  44.) 

Silver  fluomanganate,  Ag2Mn2F8+14H2O. 
(Christensen,  J.  pr.  (2)  34.  41.) 

Sodium  fluomanganate,  4NaF,  Mn2F6. 
Decomp.  by  much  H2O.    (Christensen.) 

Zinc  fluomanganate,  2ZnF2,  Mn2F6+8H2O. 
Sol.  in  H2O.    (Christensen.) 

Fluomolybdic  acid. 

See  Fluoxyhypomolybdic,  and  Fluoxymolyb- 
dic  acids. 

Fluopalladous  acid. 

Potassium  fluopalladite, 
SI.  sol.  in  H2O. 

Sodium  fluopalladite. 

SI.  sol.  in  H2O.     (Berzelius.) 

Fluoperboric  acid. 

Ammonium  fluoperborate, 

NH4OOB(F)OOB(F)OONH4. 
Ppt.     Insol  in  ether.     (Petrenko,   C.  C. 
1902,  I.  1191.) 

Potassium  fluoperborate,  K4B4F4On+H2O. 

Dry  salt  is  rather  stable. 

Easily  sol.  in  H2O.  Aqueous  solution 
decomp.  rapidly  when  warmed;  at  ordinary 


346 


FLUOPERURANIC  ACID 


temp,  the  decomp.  proceeds  slowly.     Insol. 
in  alcohol.      (Melikoff,   B.    1899,   32.   3350. 

KOOB(F)OOB(F)OK  +  13^H2O.      Ppt. 
Insol.  in  ether.     (Petrenko,   C.  C.  1902,  I. 
1191;  J.  Russ,  phys.  chem.  Soc.  34.  37.) 

Fluopemranic  acid. 

Potassium    fluoperuranate,    K4U4FfiOi5  + 
4H20=3U04KF,  U03F2,  KF+4H20. 
Ppt.    (Lordkipanidse,  C.  C.  1900,  II.  525. 

Sodium  fluoperuranate,   U04NaF+5H2O. 
Ppt.    (Lordkipanidse,  C.  C.  1900,  II.  525.) 

Fluophosphamide,  PF3(NH2)2. 

Sol.  in  H2O.      (Poulenc,  A.  ch.    (6)   24. 

566.) 

Fluophosphoric  acid. 

Monoc&sium    wowofluophosphate, 

P(OH)3(OCs)F. 

Like  the  K  salt.    (Weinland,  Z.  anorg.  1899, 
21.  48.) 

Mowopotassium  wonofluophosphate, 

P(OH)3(OK)F. 

Sol.  in  40%  HF+Aq;  decomp.  in  the  air. 
(Weinland,  Z.  anorg.  1899,  21.  44.) 

Potassium  wowofluophosphate, 

KHF.PO3+H2O. 

Decomp.  by  H2O;  unstable.     (Weinland, 
B.  1898,  31.  124-125.) 

Moworubidium  wonofluophosphate, 

P(OH)3(ORb)F. 

Sol.    in    40%    HF+Aq.      (Weinland,    Z. 
anorg.  1899,  21.  47.) 

Rubidium  raonofluophosphate, 

RbHFPO3+H2O. 

Decomp.  by  H2O.    (Weinland,  B.  1898,  31. 
124.) 

Fluoplatinic  acid. 

Ammonium  fluoplatinate. 

Secomp.  by  H2O  to  a  sol.  acid,  and  an  insol. 
basic  salt.    Insol.  in  alcohol.     (Berzelius.) 

Potassium  fluoplatinate. 

Deliquescent.    Insol.  in  alcohol.    Decomp. 
by  H2O.    (Berzelius.) 

Sodium  fluoplatinate. 

Decomp.  by  H2O.     (Berzelius.) 

Fluor-  and  Fluoro-. 
See  Fluo-. 


Fluorhydric  (Hydrofluoric)  acid,  HF  or 
H2F2. 

Attracts  H2O  from  air  with  great  avidity. 
Very  sol.  in  H2O  with  evolution  of  much  heat. 

Sat.  solution  has  sp.  gr.  1.25.    (H.  Davy.) 

On  boiling  the  aqueous  solution  an  acid  of 
constant  composition  is  obtained,  which  boils 
at  120°,  has  sp.  gr.  1.15,  and  contains  35.37% 
HF  (Bineau,  A.  ch.  (3)  7.  257.)  The  residual 
acid  after  boiling  contains  36  to  38%  HF,  and 
by  standing  over  CaO  gives  off  HF  until  an 
acid  containing  32.5  to  32.7%  HF  is  formed. 
Weaker  acids  increase  their  strength  to  32.2  to 
32.4%  HF,  while  an  acid  containing  32.5% 
HF  remains  unchanged.  (Roscoe,  A.  116. 
218.) 

Does  not  attack  gutta-percha.  Sol.  in 
H2S04. 

Sp.  gr.  of  HF+Aq  at  15°. 


Sp.  gr. 

%  HF 

Sp.  gr. 

%HF 

Sp.  gr. 

%  HF 

1.01 

2.90 

1.10 

29.00 

1.19 

55.10 

1.02 

5.80 

1.11 

31.90 

1.20 

58.00 

1.03 

8.70 

1.12 

34.80 

1.21 

60.90 

1.04 

11.60 

1.13 

37.70 

1.22 

63.80 

1.05 

14.50 

1.14 

40.60 

1.23 

66.70 

1.06 

17.40 

1.15 

43.50 

1.24 

69.60 

1.07 

20.30 

1.16 

46.40 

1.25 

72.50 

1.08 

23.20 

1.17 

49.30 

1.09 

26.10 

1.18 

52.20 

(Hart,  J.  Anal.  Ch.  3.  372.) 
Sp.  gr.  of  HF+Aq  at  ord.  temp. 


Deg.  Baum6 

Sp.  gr. 

%  HF 

1 

1.0069 

2.32 

2 

1.0139 

4.04 

3 

1.0211 

5.76 

4 

1  .  0283 

7.48 

5 

1  .  0356 

9.20 

6 

1  .  0431 

10.92 

7 

1  .  0508 

12.48 

8 

1  .  0583 

14.04 

9 

1.0661 

15.59 

10 

1.074 

17.15 

11 

1.082 

18.86 

12 

.0901 

21.64 

13 

.0983 

24.42 

14 

.1067 

27.20 

15 

.1152 

29.98 

16 

.1239 

32.78 

17 

.1326 

35.15 

18 

.1415 

37.53 

19 

.1506 

39.91 

20 

.1598 

42.29 

21 

.1691 

44.67 

22 

.1786 

47.04 

23 

.1883 

49.42 

24 

.1981 

51  .  57 

25 

.2080 

53.72 

26 

.2182 

55.87 

27 

.2285 

58.02 

FLUOSELENATE,  RUBIDIUM 


347 


Sp.  gr.  of  HF+Aq  at  ord.  temp.  —  Continued. 

Aq.  solution  of  sp.  gr.  1.138  at  18°  contains 

43.2%  HF  and  has  a  constant  bpt.  of  111° 

Deg.  Baum6 

Sp.  gr. 

%  HF 

at  750  mm.     (Deussen,  Z.  anorg.  1906,  49. 

28 
29 
30 
31 

1.2390 
1.2497 
1  .  2605 
1.2716 

60.17 
62.32 
64.47 
66.61 

297.) 
The  strongest  acid  that  can  be  obtained 
by  distillation  contains  48.17%  HF  and  boils 
at  125-125.5°.    (Gore.) 

32 

1  .  2828 

68.76 

33 

1.2943 

70.91 

Fluorides. 

34 
35 
36 
37 
38 

1.3059 
1.3177 
1.3298 
1  .  3421 
1.3546 

73.06 
75.21 
77.36 
79.51 
81.66 

The  alkali  fluorides,  also  AgF  and  SnF2, 
are  sol.  in  H2O;  the  fluorides  of  Fe,  Sr,  and 
Cd  are  si.  sol.;  the  others  are  insol.  in  H2O. 

Most  fluorides  are  sol.  in  acids,  especially  HF 

i  \  n 

39 

40 

1.3674 
1  .  3804 

83.81 
85.96 

+Aq. 
Insol.  in  liquid  NHs.     (Franklin,  Am.  Ch. 
T    18Q8   20   892  ") 

41 

1  .  3937 

88.10 

tl  .    J.Ot7Oj    *iw»    '^—i-j.J 

See  under  each  element. 

42 

1  .  4072 

90.24 

43 

1.4211 

92.39 

44 

1  .  4350 

94.54 

Fluorine,  F2. 

45 

1  .  4493 

96.69 

J        • 

Decomposes  H2O  and  all  organic  solvent 

(Eckelt,  Ch.  Z.  1898,  22.  225.) 

with  great  violence.    (Moissan,  C.  R.  103.  202 

and  256.) 

Sp. 

gr.  of  HF+Aq  at  0°. 

Liquified  at  —  185°  to  a  yellowish  liquid 
which  does  not  dissolve  glass  nor  ignite  cooled 

%  HF 

Sp.  gr. 

%  HF 

Sp.  gr. 

Si,  B,  C,  S,  P,  or  Fe.    (Moissan,  C.  R.  1897, 

0.484 

1.005 

71.73 

1.262 

124.  1202-1204.) 

1.504 

1.009 

72.21 

1.260 

2.48 

1.012 

78.05 

1.260 

Fluomolybdic  acid. 

4.80 

1.017 

84.27 

1.235 

7.75 
15.85 

1.035 
.065 

87.72 
88.11 

1.212 
1.210 

Ammonium    fluomolybdate,     (NH4)MoF4  + 

24.47 

.097 

88.82 

1.207 

±l2vy. 

28  48 

110 

89  02 

1  202 

Somewhat  more  sol.  in  H2O  thau  the  K  salt. 

29.83 

.120 

89.15 

1.200 

Hydrolysed  by  H2O.    (Rosenheim,  Z.  anorg. 

34.23 
38.50 

.130 
1.145 

89.82 
90.20 

1.190 
1.185 

1905,  46.  321.) 
(NH4)3Mo2F9+2H2O.    (Rosenheim.) 

41.00 

1.155 

90.64 

.175 

41.15 
41.92 
47.52 

1.155 
1.157 
1.182 

91.04 
92.09 
92.81 

.165 
.152 
.135 

Potassium  fluomolybdate,  KMoF4+H2O. 
Nearly  insol.  in  H2O.    (Rosenheim.) 

48.49 

1.187 

92.91 

.130 

50.97 
55.09 

1.200 
1.217 

94.26 
95.84 

1.095 
1.065 

Fluoselenic  acid. 

55.39 

1.220 

97.50 

1.035 

57.66 

1.230 

98.22 

1.022 

Ammonium  monofluoselenate, 

61.66 

1.245 

100.05 

1.0005 

Se03(OH)F(NH4)2. 

65.19 

1.255 

Not  hygroscopic. 

Easily  sol.  H2O  with  decomp. 
Sol.  in  HF.    (Weinland,  Z.  anorg.  1899,  21. 

(Hill,  Roy. 

Soc.  Proc.  1909,  83.  A.  144.) 

Sp. 

gr.  of  HF+Aq  at  18°. 

58.) 

%  HF 

Sp.  gr. 

rnpotassium  difluocftselenate,  Se2O7F2K3H  + 

0  484 

1.003 

H2O. 

1  504 

005 

Decomp.  in  the  ajr;  sol.  in  H2O  with  de- 

2^48 

^009 

comp.;  sol.  in  HF.    (Weinland.) 

4.80 

.017 

7.75 
15.85 

.028 
.058 

Tn'rubidium  cfofluocftselenate,  Se2O7F2Rb3H 

24.4' 

r 

.087 

i"Xi2L/. 

29  '.  83 

103 

Decomp.  in  the  air;  sol.  in  H2O  with  de- 

comp.; sol.  in  HF.     (Weinland,   Z.   anorg. 

(Hill.) 

1899,  21.  57.) 

348 


FLUOSILICIC  ACID 


Fluosilicic  acid,  H2SiF6. 
Sp.  gr.  of  H2SiF6+Aq  at  17.5°  (H2O  at 
17.5°  =  1.000). 

1   pt.   BaSiF6   dissolves  in   306   pts.   sat. 
NH4Cl+Aq  at  22°;  in  361  pts.  15%  solution 
of  NF4C1;  in  563  pts.  sat.  boiling  NaCl+Aq; 
in  349  pts.  10%  solution  of  NaCl  at  boiling 
temp.;  in  2185  pts.  10%  solution  of  NaCl  at 
20°;  in  1140  pts.  5%  solution  of  NaCl  at  20°. 
(Stolba.) 
Nearly  absolutely  insol.  in  alcohol.     (Fre- 
senius.) 

Solubility  in  a  mixture  of  H2O,  alcohol  (96%). 
HCl+Aq    (20%),    H2SiF6+Aq    (3.7%). 
1  pt.  BaSiFc  is  sol.  in  pts.  of  solutions  of 
given  composition. 

%  H2SiF6 

Sp.  gr. 

%  H2SiF6 

Sp.  gr. 

2 

4 
6 
8 
10 
12 
14 
16 
18 

1.0161 
1.0324 
1.0491 
1  .  0661 
1  .  0834 
1.1011 
1.1190 
1.1373 
1.1559 

20 
22 
24 
26 
28 
30 
32 
34 

1.1748 
1.1941 
.2136 
.2335 
.2537 
.2742 
.2951 
.3162 

H20 

Alcohol 

HCl+Aq 

H2SiF6 
+Aq 

BaSiFe 

(Stolba,  J.  pr.  90.  193.) 

+2H2O.     Very  deliquescent,  and  sol.  in 
H2O.     (Kessler,  C.  R.  90.  1285.)     Solution 
decomp.  into  HF  and  SiF4  on  evaporation, 
when  it  becomes  concentrated. 

Fluosilicates. 
Most  of  the  fluosilicates  are  sol.  in  H20,  but 
the  alkali  salts  (especially  K)  and  the  Ba  salt 
are  only  si.  sol.  in  H2O. 

50 
74.1 
70.8 
77.95 
73.0 
97.09 
75.0 

50 
25 
25 
20 
25 
0 
25 

0 
0.9 
4.2 
0.9 
0.9 
1.25 
0 

0 
0 
0 
1.15 
1.1 
1.66 
0 

37,219 
5,263 
2,860 
39,061 
70,679 
3,247 
16,914 

(Fresenius,  Z.  anal.  29.  143.)  • 

Aluminum  fluosilicate,  Al2(SiF6)3. 

Easily  sol.  in  H2O.  After  evaporating  to 
dryness,  the  residue  is  slowly  but  completely 
sol.  in  H2O.  (Deyille,  A.  ch.  (3)  61.  327.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

Aluminum  fluosilicate  silicate,  Al2SiFi0, 

5AI2Si05. 
Min.  Topaz.    Insol,  in  acids. 

Ammonium  fluosilicate,  (NH4)2SiF6. 

Sol.  in  5.38  pts.  H2O  at  17.5°  to  form  a  solu- 
tion of  1.0961  sp.  gr.;  sol.  in  1.8  pts.  hot 
H20;  sol.  in  45.5  pts.  alcohol  of  31%.  (Stolba, 
C.  C.  1877.  418.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

3NH4F,  SiF4  =  (NH4)2SiI6,  NH4F.  Sol.  in 
H2O.  (Marignac,  Ann.  Min.  (5)  15.  221.) 

Barium  fluosilicate,  BaSiF6. 

Sol.  in  3802  pts.  cold  H2O.  (Fresenius,  A. 
59.  120.) 

Sol.  in  3731  pts.  H2O  at  17.5°;  in  3315  pts. 
at  21°;  in  1175  pts.  at  100°.  (Stolba,  J.  pr.  96. 
22.) 

Sol.  in  640-733  pts.  H20  containing  a  little 
HC1.  (Fresenius.) 

488  pts.  HCl+Aq  containing  4.25%  HC1 
dissolve  1  pt.  at  22°.  (Stolba.) 

More  sol.  in  HNO3+Aq  than  in  H2O. 
(Fresenius.) 

272  pts.  HNO3+Aq,  containing  8%  N2O5, 
dissolve  1  pt.  at  22°.  (Stolba.) 

1  pt.  BaSiF6  dissolves  in  428  pts.  sat. 
NH4Cl+Aq;  in  589  pts.  sat.  NH4Cl+Aq  + 
2  vols.  H2O.  (Mallet,  Sill.  Am.  J.  (2)  28.  48.) 


Cadmium  fluosilicate,  CdSiF6+6H2O. 

Extremely  sol.  in  H2O.  Easily  sol.  in  50% 
alcohol.  (Engelskirchen,  Dissert.  1903.) 

Caesium  fluosilicate,  Cs2SiF6. 

Sol.  in  166  pts.  H2O  at  17°,  and  much  less 
h2t  H2O.  Insol.  in  alcohol.  (Preis,  J.  pr. 
103.  410.) 

Calcium  fluosilicate,  CaSiF6+2H20. 

SI.  sol.  in,  and  partly  decomp.  by  H2O.  Sol. 
in  HF  and  HCl+Aq.  Sol.  in  fluosilicic  acid 
without  decomp.  Easily  sol.  in  60%  alcohol. 
(Fleischer.) 

Cerium  fluosilicate. 

Very  difficulty  sol.  in  H2O,  acetic,  or  fluo- 
silicic acids.  Insol.  in  alcohol.  (Stolba,  C. 
C.  1874.  130.) 

Chromium  fluosilicate. 
Deliquescent.    (Berzelius.) 
Efflorescent.    Sol.  in  H20.    (Berlin.) 

Cobaltous  fluosilicate,  CoSiF6+6H2O. 
Easily  sol.  in  H20.    (Berzelius.) 

Cuprous  fluosilicate,  Cu2SiF6. 

Insol.  in  H2O.    (Berzelius,  Pogg.  1.  199.) 

Cupric  fluosilicate,  CuSiF6+6H2O. 

Deliquescent  in  moist,  efflorescent  in  dry 
air. 

Sol.  in  0.428  pt.  H2O  at  17°.  Sp.  gr.  of 
solution  sat.  at  17°  =  1.6241. 

Sol.  in  17.5  pts.  alcohol  of  62  vol.  %  at  20°; 
in  150  pts.  of  85%  at  20°;  in  617  pts.  of  92% 
at  20°.  (Stolba,  J.  pr.  102.  7.) 


FLUOSILICATE,  POTASSIUM 


349 


Insol.  in  methyl  acetate.     (Naumann,  B, 
1909,  42.  3790.) 
Contains  §1A  H2O.    (Stolba.) 
+5^H2O.    (Knop  and  Wolf.) 

Cupric  fluosilicate  phosphate,  CuSiF6, 

Cu3(P04)2. 

Insol.  in  H2O,  but  easily  sol.  in  dil.  HC1  + 
Aq.  (Thorpe  and  Rodger,  Chem.  Soc.  65. 
320.) 

Glucinum  fluosilicate. 
Known  only  in  solution. 

Iron  (ferrous)  fluosilicate,  FeSiF6+6H20. 
Easily  sol.  in  H2O.    (Berzelius.) 

Iron  (ferric)  fluosilicate,  Fe2(SiF6)3. 
Sol.  in  H2O.    (Berzelius.) 

Lead  fluosilicate,  PbSiF6+2H2O. 

Deliquescent.    Easily  sol.  in  H2O. 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

+4H2O.    (Marignac.) 

Lithium  fluosilicate,  Li2SiF6+2H2O. 

100  pts.  H2O  at  17°  dissolve  73  pts.  crystal- 
line salt.  (Marignac.) 

100  pts.  cold  H2O  dissolve  52.6  pts.  crystals. 

Sol.  in  dil.  alcohol.    (Stolba,  J.  pr.  91.  456.) 

100  pts.  alcohol  of  46  vol.  %  dissolve  about 
4  pts.,  and  100  pts.  alcohol  of  79  vol.  %  dis- 
solve about  0.4  pt.  crystals.  (Stolba,  Z.  anal. 
3.  311.) 

Insol.  in  ether  or  benzene. 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1904,37.3601.)" 

Magnesium  fluosilicate,  MgSiF6+6H2O. 

Efflorescent.  Sol.  in  1534  pts.  cold  H2O, 
forming  a  solution  of  1.235  sp.  gr.  at  17.5°. 
Separates  out  SiO2  on  warming,  which  nearly 
all  redissolves  on  cooling.  (Stolba,  C.  C. 
1877.  578.) 

Magnesium  fluosilicate   silicate,   Mg5Si2Fi8, 

.TMg5Si209. 

Min.  Humite;  Chondrodite.  Gelatinises 
with  HC1,  or  H2SO4+Aq. 

Manganous  fluosilicate,  MnSiF6+6H2O. 
Sol.  in  H2O.    (Marignac,  J.  pr.  83.  202.) 
100    pts.    dissolve    in    71.4   pts.    H2O    at 
17.5°,  and  sp.  gr.  of  solution  =  1.44825.  Much 
more  sol.  in  hot  H2O,  and  less  sol.  in  alcohol, 
the  stronger  the  alcohol.    (Stolba,  C.  C.  1883. 
292.) 


Mercurous  fluosilicate,  Hg2SiF6. 

SI.  sol.  in  H2O  without  decomp.  (Lemaire, 
C.  C.  1897,  I.  1046.) 

+2H20.  SI.  sol.  in  H2O.  More  easily  sol. 
in  acidified  H2O,  but  precipitated  by  HC1  + 
Aq.  (Berzelius.) 

Mercuric  fluosilicate,  basic,  HgSiF6,  HgO  + 

3H2O. 

Decomp.  by  H2O,  but  sol.  in  weakest  acids- 
(Berzelius,  Pogg.  1.  200.) 

Mercuric  fluosilicate,  HgSiF6+6H2O. 

Deliquescent,  and  easily  sol.  in  H20. 
(Finkener,  Pogg.  111.  246.) 

Nickel  fluosilicate,  NiSiF6+6H2O. 

Easily  sol.  in  H2O.  (Marignac,  Ann.  Min. 
(5)  16.  262.) 

Potassium  fluosilicate,  K2SiF6. 

Sol.  in  833.1  pts.  H2O  at  17.5°,  and  104.8 
pts.  at  100°.  (Stolba,  J.  pr.  103.  396.)  Sol. 
in  3800  pts.  cold,  and  more  easily  sol.  in  hot 
H2O.  (Fresenius.) 

More  sol.  in  HCl+Aq  than  in  H2O. 

Sol.  in  337  pts.  HCl+Aq  of  26.5%  at  14°; 
in  307  pts.  of  25.7%  at  15°;  in  340  pts.  of  14.1 
%  at  14°;  in  303  pts.  of  13.6%  at  15°;  in  327 
pts.  of  9.6%  at  14°;  in  313  pts.  of  9.2%  at 
15°;  in  376  pts.  of  2.7%  at  14°;  in  319  pts.  of 
2.4%  at  15°;  in  409  pts.  of  1.8%  at  14°. 
(Stolba,  1.  c.) 

Sol.  in  428  pts.  sat.,  and  589  pts.  dil. 
NH4Cl+Aq.  (Mallet.) 

Much  less  sol.  in  K2SO4,  KNO3,  or  KC1+ 
Aq,  but  more  sol.  in  NH4Cl+Aq  than  in  H2O. 
(Stolba.) 

Sol.  in  24,066  pts.  K2SO4+Aq  containing 
9.92%  K2SO4  at  17°;  in  17,858  p!s.  containing 
6%  at  18°;  in  19,530  pts.  containing  5%  at 
17°;  in  10,721  pts.  containing  1%  at  17°. 

Sol.  in  125,000  pts.  KNO3+Aq  containing 
18.4%  KNO3  at  15°;  in  43,478  pts.  containing 
8.7%  at  15°;  in  1735  pts.  containing  8.8%  at 
100°;  in  35,814  pts.  containing  4.3%  at  15°; 
in  10,203  pts.  containing  1.00%  at  15°. 

Sol.  in  40,070  pts.  KCl+Aq  containing  25% 
KC1  at  17°;  in  38,352  pts.  containing  18.4% 
at  17°;  in  41,254  pts.  containing  13.4%  at  14°; 
in  24,032  pts.  containing  6.7%  at  12°;  in  1200 
pts.  containing  0.65%  at  17°;  in  1095  pts. 
containing  0.45%  at  18°. 

Sol.  in  358  pts.  NH4Cl+Aq  containing  26.3 
%NH4C1  at  17°;  in  306  pts.  containing  15% 
at  15°;  in  339  pts.  containing  10%  at  15°;  in 
436  pts.  containing  5%  at  15°.  (Stolba,  J.  pr. 
103.  306.) 

Insol.  in  liquid  CO2.  (Biichner,  Z.  phys. 
Ch.  1906,  54.  674.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  ch.  J. 
1898,  20.  829.) 

Completely  pptd.  from  aqueous  solution  by 
an  equal  vol.  of  alcohol. 


350 


FLUOSILICATE,  RUBIDIUM 


SI.   sol.   in   benzbnitrile. 
1914,  47.  1369.) 

Insol.  in  methyl  acetate. 
1909,  42.  3790.) 


(Naumann,   B. 
(Naumann,  B. 


Rubidium  fluosilicate,  Rb2SiF6. 

Sol.  in  625  pts.  H2O  at  20°,  and  73.05-74.5 
pts.  at  100°.  More  sol.  in  acidified  water. 
Insol.  in  alcohol.  (Stolba,  J.  pr.  101.  1.) 

Insol.  in  H2O.  (Eggeling,  Z.  anorg.  1905, 
46.  175.) 

Less  sol.  in  H2O  than  K2SiF6.  (Gossner, 
Zeit.  Kryst.  1904,  38.  149.) 

Silver  fluosilicate,  Ag2SiF6+4H2O. 

Deliquescent.  Easily  sol.  in  H2O.  (Marig- 
nac,  Ann.  Min.  (5)  15.  221.) 

Sodium  fluosilicate,  Na2SiF6. 

Much  more  sol.  in  H2O  than  K2SiF6,  es- 
pecially in  hot  H2O.  Addition  of  acid  does 
not  increase  solubility.  (Berzelius.) 

Sol.  in  153.3  pts.  H2O  at  17.5°,  and  40.66 
pts.  at  100°.  Easily  forms  supersaturated 
solutions.  (Stolba,  Z.  anal.  11.  199.) 

Much  less  sol.  in  NaCl+Aq  than  in  H2O. 
(Stolba,  J.  pr.  1865  (1)  96.  26.) 

Precipitated  completely  from  aqueous  solu- 
tion by  alcohol.  (Rose.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Strontium  fluosilicate,  SrSiF6+2H2O. 

Sol.  in  cold  H2O,  but  decomp.  somewhat  on 
heating.  Sol.  in  31.06  pts.  H2O.  (Fresenius.) 

Easily  sol.  in  acidified  H2O  without  de- 
comp. Sol.  in  alcohol. 

Solubility  in  a  mixture  of  H2O,  alcohol  (96%), 
HCl+Aq  (20%),  H2SiF6+Aq  (3.7%). 
1  pt.  SrSiF«  is  sol.  in  pts.  of  solutions  of 
given  composition. 


H20 

Alcohol 

HCl+Aq 

H2SiF6 

+Aq 

SrSiFa 

50 

50 

0 

0 

15.29 

74.1 

25 

0 

0 

82.93 

70.8 

25 

4.2 

0 

50.9 

77.95 

20 

0.9 

1.15 

55.0 

73 

25 

0.9 

1.1 

82.97 

75 

25 

0 

0 

147.4 

95.24 

0 

2.04 

2.72 

7.3 

(Fresenius,  Z.  anal.  29.  143.) 

Thallous  fluosilicate,  Tl2SiF6-f-2H2O. 

Very   easily   sol.   in   H2O.      (Kuhlmann.) 

Thorium  fluosilicate,  Th(OH)2SiF6  (?). 
(Cleve.) 

Tin  (stannic)  fluosilicate,  SnF4,  SiF4. 
Very  easily  sol.  in  H2O.     (Berzelius.) 


Uranyl  fluosilicate. 

Very  si.  sol.  in  acids.    (Berzelius.) 

Sol.  in  alcohol.     (Stolba,  Z.  anal.  3.  71.) 

Vanadium  fluosilicate. 

Deliquescent.  Sol.  in  H2O.  (Guyard,  Bull. 
Soc.  (2)  25.  352.) 

Yttrium  fluosilicate. 

Insol.   in   pure,    sol.   in   acidified   H2O. 
(Berzelius.) 

Zinc  fluosilicate,  ZnSiF6+6H2O. 

Very  easily  sol.  in  H2O.     (Berzelius.) 

Zirconium  fluosilicate. 

Sol.  in  H2O.  Solution  clouds  up  on  boiling. 
(Berzelius.) 

Fluostannic  acid. 

Ammonium  fluostannate,  (NH4)2SnF6. 

Sol.  in  H2O.  (Marignac,  Ann.  Min.  (5)  15. 
224.) 

4NH4F,SnF4.   Sol.  in  H2O.    (Marignac.) 

Barium  fluostannate,  BaSnF6. 

Slowly  sol.  in  H2O. 

+3H2O.  Sol.  in  18  pts.  H2O  at  18°. 
(Marignac,  Ann.  Min.  (5)  15.  246.) 

Decomp.  by  warming  with  H2SO4  with 
evolution  of  HF.  (Emich,  M.  1904,  25.  1912.) 

Calcium  .fluostannate,  CaSnF6+2H2O. 

Sol.  in  H2O.  (Marignac,  Ann.  Min.  (5)  15. 
250.) 

Cadmium  fluostannate,   CdSnF6+6H2O. 
Sol.  in  H2O.    (Marignac.) 

Cobaltous    fluostannate,    CoSnF6+6H2O. 
(Gossner,  Zeit.  Kryst.  1907,  42.  482.) 

Cupric  fluostannate,  CuSnF6+4H2O. 

Not  deliquescent.  (Marignac,  Ann.  Min. 
(5)  15.  291.) 

Lithium  fluostannate,  Li2SnF6-f-2H2O. 
Sol.  in  H2O.    (Marignac,  Ann.  Min.  (5)  15. 

242.) 

Magnesium  fluostannate,  MgSnF6+6H2O. 

Not  deliquescent.  Sol.  in  H2O.  (Marig- 
nac, Ann.  Min.  (5)  15.  256.) 

Manganous  fluostannate,  MnSnF6+6H20. 
Slowly  efflorescent.    (Marignac.) 

Nickel  fluostannate,  NiSnF6+6H2O. 

Sol.  in  H2O.    (Marignac.  Ann.  Min.  (5)  15. 

262..) 


FLUOTELLURATE,  AMMONIUM 


351 


Potassium  fluostannate,  K2SnF6+H2O. 

Two  modifications — (a)  Thin  plates.  Sol. 
in  2.3  pts.  H2O  at  100°,  and  in  15-16  pts.  at 
18°.  (Marignac.) 

(b)  Octahedra.  Sol.  in  3  pts.  HoO  at  100°, 
and  27  pts.  at  18°.  (Marignac.) 

Sol.  in  hot  H2O.  Can  be  cryst.  from  hot 
H2O.  With  cone.  H2SO4,  HF  is  evolved. 
(Emich,  M.  1904,  25.  911.) 

Potassium  hydrogen  fluostannate,  3KF,  HF, 
SnF4. 

Sol.  in  H2O.    (Marignac.) 

Silver  fluostannate,  Ag2SnF6+4H2O. 

SI.  deliquescent.  Easily  sol.  in  H2O. 
(Marignac.) 

Sodium  fluostannate,  Na4SnF6. 

Sol.  in  18-19  pts.  H2O  at  20°.    (Marignac.) 

Strontium  fluostannate,  SrSnF6+2H2O. 
Sol.  in  5.5  pts.  H2O  at  18°.    (Marignac.) 

Zinc  fluostannate,  ZnSnF6+6H2O. 
Sol.  in  H2O.     (Marignac.) 

Fluosulphonic  acid,  HSO3F. 
See  Sulphuryl  hydroxyl  fluoride. 

Ammonium  fluosulphonate,  FSO3NH4. 

Easily  sol.  in  H2O  from  which  it  can  be 
cryst. 

Sol.  in  ethyl  alcohol,  more  sol.  in  methyl 
alcohol.  Can  be  cryst.  from  abs.  alcohol. 
(Traube,  B.  1913,  461  2528.) 

Sodium  fluosulphonate,  FSO3Na. 
Hydroscopic. 
Sol.  in  alcohol  and  acetone.    (Traube.) 

Fluosulphuric  acid. 

Tn'caesium    c^fluocfo'sulphate,    S2O7F2Cs3H+ 
H2O. 

As  the  K  salt.  (Weinland,  Z.  anorg.  1899, 
21.  53.) 

Tn'potassium  c&fluoeftsulphate, 

S207F2K3H+H20. 

Sol.  in  HF;  quite  stable  in  air;  sol.  in  H2O 
with  decomp.  (Weinland,  Z.  anorg.  1899, 

Tn'rubidium    difluodisulphate,   S2O7R2Tb3H 
+H2O. 

Sol.  in  HF.  (Weinland,  Z.  anorg.  1899,  21. 
53.) 

Fluotantalic  acid. 

Ammonium  fluotantalate,    (NH4)2TaF7. 
Very  sol.  in  H2O.    (Marignac,  A.  ch.  (4)  9. 

-  272.) 


(NH4)3TaF8.  (Balke,  J.  Am.  Chem.  Soc. 
1905,  27.  1151.) 

Caesium  fluotantalate,  CsTaF6. 
Can  be  recryst.  from  HF+Aq.     (Balke.) 
Cs2TaF7.    Can  not  be  recryst.  from  H2O  as 

it  tends  to  go  into  CsF,  TaF6.     (Balke,  J. 

Am.  Chem.  Soc.  1905,  27.  1151.) 

ISCsF,  TaF5.    SI.  sol.  in  H2O.     (Penning- 

ton,  J.  Am.  Chem.  Soc.  1896, 18.  59.) 

Calcium  fluotantalate. 
Difficulty  sol.  in  H2O      (Berzelius.) 

Cupric  fluotantalate,  CuTaF7+4H2O. 

Deliquescent.  Easily  sol.  in  H2O.  (Marig- 
nac, A.  ch.  (4)  9.  294. 

Lead  fluotantalate. 

Difficulty  sol.  in  H2O.     (Berzelius.) 

Lithium  fluotantalate,  LiF,   TaF8+2H2O. 

Can  be  recryst.  from  cone.  HF.  (Balke,  J. 
Am.  Chem.  Soc.  1905,  27.  1143.) 

Potassium  fluotantalate,  K2TaF7. 

SI.  sol.  in  cold,  much  more  easily  in  hot 
H2O.  Decomposes,  with  formation  of  a 
white  precipitate  on  boiling.  (Berzelius.) 

Much  more  sol.  in  HF+Aq.  1  pt.  of  the 
salt  is  sol.  in  200  pts.  H2O  containing  a  trace 
of  HF,  and  in  150-160  pts.  of  H2O  containing 
a  little  more  HF.  (Marignac.  A.  ch.  (4)  9. 
267.) 

Potassium  hydrogen  fluotantalate,  KF,  HF, 

TaF6  (?). 
Sol.  in  H2O.    (Berzelius.) 

Rubidium  fluotantalate,  Rb2TaF7. 

Sol.  in  HF+Aq.  (Pennington,  J.  Am.  Ch. 
Soc.  1896,  18.  58.) 

3RbF,  2TaF5.  (Balke,  J.  Am.  Chem. 
Soc.  1905,  27.  1151.) 

Sodium  fluotantalate,  3NaF,  TaF5, 
Easily  sol.  in  H2O. 
Na2TaF7+H2O.    Sol.inH2O.    (Marignac.) 

Thallous  fluotantalate,  Tl2TaF7. 

Sol.  in  HzO.  On  boiling  the  aqueous  solu- 
tion tantalic  acid  separates. 

Decomp.  by  cone.  H2SO4.  Difficultly 
sol.  in  cold,  easily  sol.  in  hot  HF.  (Ephraim. 
B.  1909,  42.  4461.) 

Zinc  fluotantalate,  ZnTaF7+7H2O. 

Very  deliquescent.  Sol.  in  H2O.  (Marig- 
nac, A.  ch.  (4)  9.  249.) 

Fluotelluric  acid. 

Ammonium  fluotellurate,  NH4TeF5+H2O. 

Decomp.  by  H2O.  (Hogbom,  Bull.  Soc. 
(2)  35.  60.) 


352 


FLUOTELLURATE,  BARIUM 


Barium  fluotellurate,    Ba(TeF5)2+H2O. 
As  above. 

Potassium  fluotellurate,  KTeF5. 

As  above. 

TeO3F2K2+3H2O.  Stable  in  dry  air;  only 
si.  sol.  in  H2O  with  decomp.;  sol.  in  HF. 
(Weinland,  Z.  anorg.  1899,  21.  61.) 

Rubidium  ^fluotellurate,  Te03F2Rb2+3H2O. 
SI,  sol.  in  H2O  with  decomp.  ,  Sol.  in  HF. 
(Weinland,  Z.  anorg.  1899,  21.  62.) 

Fluotitanic  acid. 

Known  only  in  solution  as  titanium  hydro- 
gen fluoride. 

Ammonium  fluotitanate,  (NH4)2TiF6. 
Sol.  in  H2O.     (Marignac.) 
3NH4F,  TiF4.     Sol.  in  H2O.     (Marignac.) 

Ammonium  fluosegtutitanate,  6NH4F,  Ti2F'6. 

Easily  sol.  in  H2O.  SI.  sol.  in  NH4F+Aq. 
(Petersen,  J.  pr.  (2)  40.  54.) 

Insol.  in  NH4F+Aq.  (Piccini,  C.  R.  97. 
1064.) 

4NH4F,  Ti2F6.  Properties  as  the  cor- 
responding K  salt.  (Piccini,  B.  18.  257  R.) 

Barium  fluotitanate,  BaTiF6. 

Very  si.  sol.  in  H2O.  More  easily  sol.  in 
dil.  HNO3  or  HC1.  (Engelskirchen,  Dissert. 
1903.) 

+  y2B.2O.    (Emich,M.1904,25.907.) 

Cadmium   fluotitanate,   CdTiF6+6H2O. 

Extremely  sol.  in  H2O.  Easily  sol.  in  50% 
alcohol.  (Engelskirchen,  Dissert.  1903.) 

Caesium  fluotitanate,  Cs2TiF6. 

More  sol.  in  hot  than  cold  H2O  and  much 
more  sol.  than  the  Rb  comp.  (Engels- 
kirchen, Dissert.  1903.) 

4CsF,  TiF4.  More  sol.  in  H2O  than 
Csi5TaF2o  and  is  not  decomp.  by  pure  H2O. 
(Pennington,  J.  Am.  Chem.  Soc.  1896,  18. 
60.) 

Calcium  fluotitanate,  CaTiF6+3H2O. 

Decomp.  by  pure  H2O.  Sol.  without  de- 
comp. in  acidified  H2O.  (Berzelius.) 

Separates  a  precipitate  with  cold  H2O, 
which  dissolves  on  heating.  (Marignac,  Ann. 
Min.  (5)  15.  250.) 

Cupric  fluotitanate,  CuTiF6+4H2O. 

Sol.  in  pure  H2O  with  partial  decomp.; 
easily  and  completely  sol.  in  acidified  H2O. 
(Berzelius.) 

Cupric    fluotitanate    ammonium    fluoride, 

CuTiF6,  NH4F+4H2O. 
Efflorescent.    Easily  sol.  in  H2O.    (Marig- 
nac, Ann.  Min.  (5)  15.  267.) 


Cupric    fluotitanate    potassium    fluoride, 

CuTiF6,  KF+4H2O. 
As  the  above  salt.    (Marignac.) 

Ferrous  fluotitanate,  FeTiF6+6H2O. 

Sol.  in  H2O.     (Weber,  Pogg.   120.  287.) 

Ferric  fluotitanate. 

Decomp.  by  H2O.    (Berzelius.) 

Lead  fluotitanate. 

Easily  sol.  in  H2O.    (Berzelius.) 

Lithium  fluotitanate,  Li2TiF6+2H2O. 

Very  sol.  in  H2O.  (Engelskirchen.  Dissert, 
1903.) 

Magnesium  fluotitanate,  MgTiF6+6H2O. 

Easily  sol.  in  cold  H2O.  (Marignac,  Ann. 
Min.  (5)  15.  257.) 

Nickel  fluotitanate,   NiTiF6+6H2O. 

Easily  sol.  in  H2O.     (Weber,  Pogg.  120. 

282.) 

Potassium  fluotitanate,  K2TiF6. 

Difficultly  sol.  in  cold,  much  more  easily  in 
hot  H2O. 

100  pts.  H2O  dissolve  at: 

0°     3°     6°         10°     14°     20° 
0.556  0.667  0.775  0.909  1.042  1.28  pts.  K2TiF6. 
(Marignac,  A.  ch.  (4)  8.  65.) 

Sol.  in  78.6  pts.  H2O  at  21°.  Sol.  in  acids. 
(Piccini,  Gazz.  ch.  it,  1886,  16.  104.) 

Sol.  in  78  pts.  H2O  at  20°;  9.4  pts.  at  100°. 
By  addition  of  small  amount  of  HF,  the 
solubility,  is  increased.  (Weiss  and  Kaiser, 
Z.  anorg.  1910,  65.  354.) 

Sol.  in  HF.  (Marchetti,  Z.  anorg.  1895, 
10.  66.) 

+H2O.  Much  less  sol.  in  H2O  in  presence 
of  KBr  or  KI.  (Hall,  J.  Am.  Chem.  Soc. 
1904,  26.  1246.) 

Sol.  in  H2O  or  HF  with  decomp.  (Mar- 
chetti, Z.  anorg.  1895,  10.  66.) 

Potassium  fluoses^wztitanate,  4KF,  Ti2F6. 

Scarcely  sol.  in  H2O;  sol.  in  dil.  acids. 
(Piccini,  B.  18.  257  R.) 

Rubidium  fluotitanate,  Rb2TiF6. 

Very  si.  sol.  in  cold,  somewhat  more  sol.  in 
hot  H2O.  (Engelskirchen,  Dissert.  1903.) 


Silver  fluotitanate. 
Very  deliquescent. 


(Marignac.) 


Sodium  fluotitanate,  Na2TiF6. 

Much  more  sol.  in  H2O  than  the  corre- 
sponding potassium  salt.  (Marignac,  Ann. 
Min.  (5)  15.  238.) 


FLUOXHYPOMOLYBDATE,  CUPRIC 


353 


Sodium     hydrogen     fluotitanate,     Na2TiF6, 

NaHF2. 
Sol.inH2O.    (Marignac.) 

Strontium  fluotitanate,  SrTiF6+2H2O. 

Sol.  in  cold  H2O.  Solution  clouds  up  on 
heating.  (Marignac.) 

Zinc  fluotitanate,  ZnTiF6+6H2O. 

Sol.  in  H2O.  (Marignac,  A.  ch.  (3)  60. 
304.) 

Fluovanadic  acid. 

Ammonium  fluovanadate,  3NH4F,  VF3. 

Moderately  sol.  in  H2O.  More  easily  sol. 
in  dil.  acids.  Nearly  insol.  in  alcohol  or  MF 
+Aq.  (Petersen,  J.  pr.  (2)  40.  52.) 

2NH4F,  VF3+H2O.  Easily  sol.  in  H2O. 
SI.  sol.  in  alcohol.  (Petersen.) 

NH4F,  VF3+2H2O.  As  above.  (Peter- 
son.) 

Cadmium  fluovanadate,  CdF2,  VF,+7H2O. 
Very  si.  sol.  in  H2O.    (Piccini  and  Giorgis, 
Gazz.  ch.  it.  22, 1.  89.) 

Cobalt  fluovanadate,  CoF2,  VF3-f2H20. 

Sol.  in  H2O  without  decomp.  (Petersen, 
I  c.) 

Nickel  fluovanadate,  NiF2,  VF3+2H2O. 
As  the  Co  salt.    (Petersen.) 

Potassium  fluovanadate,  2KF,  VF3+H2O. 

SI.  sol.  in  H2O;  easily  sol.  in  acids.  Insol. 
in  KF+Aq.  (Petersen,  J.  pr.  (2)  40.  51.) 

Potassium  fluovanadate  fluoxyvanadate, 

4KF,  VF3,  VOF3. 

Easily  sol.  in  H2O,  and  still  more  easily  in 
HF+Aq.  SI.  sol.- in  KF+Aq.  (Petersen,  J. 
pr.  (2)  40.  274.) 

Sodium  fluovanadate,  5NaF,  2VF3+H20. 
As  the  potassium  salt.    (Petersen.) 

Thallous  fluovanadate,  T1F,  VF3+2H2O. 

Easily  sol.  in  H2O. 

Sol.  with  decomp.  in  cone.  H2SO4,  dil. 
HNO3  or  cold  dil.  HC1. 

Insol.  in  NaOH+Aq.  (Ephraim,  B.  1909, 
42.  4460.) 

2T1F,  VF3+H2O.    Easily  sol.  in  H20. 

Sol.  in  cone.  H2S04,  dil.  HNO3,  or  cold  dil. 
HC1  with  decomp. 

Insol.    in    cold    or   hot    NaOH+Aq. 
(Ephraim,  B.  1909,  42.  4461.) 

Zinc  fluovanadate,  ZnF2,  VF,+7H2O. 

SI.  sol.  in  cold  H2O.  Decomp.  on  heating. 
(Piccini  and  Giorgis.) 


Fluoxycolumbic  acid. 

Ammonium  fluoxycolumbate,  3NH4F,  CbOF,. 

Cubic  salt.  Sol.  in  H2O.  (Marignac,  A. 
ch.  (4)  8.  38.) 

2NH4F,  CbOF3.  Lamellar  salt.  Much 
more  sol.  in  H2O  than  2KF,  CbOF3.  (M.) 

5NH4F,  3CbOF3+H20.  Hexagonal  salt. 
(M.) 

NH4F,  CbOF3.    Rectangular  salt.    (M.) 


Ammonium  fluoxycolumbate  columbiuxn  flu- 
oride, 3N1 

(Marignac.) 


>xyc 
oride,  3NH4F,  CbOF3,  CbF6. 

Cupric    fluoxycolumbate,    CuF2,    CbOF3+ 

4H2O. 

SI.  deliquescent.  Sol.  in  H2O.  (Marignac, 
A.  ch.  (4)  8.  42.) 

Potassium  fluoxycolumbate,  2KF,  CbOF8+ 
H2O. 

Sol.  in  12.5-13  pts.  H2O  afc  17-21°.  Much 
more  sol.  in  hot  H2O,  or  H2O  containing  HF. 
(Marignac.) 

3KF,  CbOF3.  Decomp.  by  H2O  into  above 
salt.  (M.) 

5KF,  3CbOF8+H20.    Sol.  in  H20.    (M.) 

4KF,  3CbOF3+  H2O.    Sol.  in  H2O.    (M.) 

3KF,  2Cb2Ofi+5H2O.  SI.  sol.  in  H2O. 
(Petersen,  J.  pr.  (2)  40.  287.) 

KF,  Cb2O6+3H2O.  SI.  sol.  in  H2O.  (Pe- 
tersen.) 

2KF,  3CbO2F.  Insol.  in  H2O.  Sol.  in  HF. 
(Kriiss  and  Nilson,  B.  20.  1689.) 

See  also  Fluoxypercolumbate,  potassium. 

Potassium  hydrogen  fluoxycolumbate,  3KF, 

HF,  CbOFs. 
Sol.  in  H2O.    (Marignac.) 

Sodium   fluoxycolumbate,   2NaF,    CbOF,-f 

2H20. 
Sol.  in  H20. 
NaF,  CbOF3+H2O.    (Marignac.) 

Zinc  fluoxycolumbate,  ZnF2,  CbOF3+6H2O. 
Sol.  in  H20.     (Marignac,  A.  ch.   (4)  8. 
41.) 

Fluoxyhypomolybdic  acid. 

Ammonium  fluoxyhypomolybdate,  MoOF», 
2NH4F. 

Decomp.  by  H2O.  (Mauro,  Gazz.  ch.  it. 
19.  179.) 

3MoOF3,  5NH4F+H20.  Decomp.  by 
H2O.  (Mauro.) 

Cupric  fluoxyhypomolybdate,  CuF2,  MoOFt+ 

4H20. 

Deliquescent.  Sol.  hi  H2O.  (Mauro, 
Real.  Ac.  Line.  1892, 1.  194.) 


354 


FLUOXYHYPOMOLYBDATE,  POTASSIUM 


Potassium  fluoxyhypomolybdate,  MoOF3 
2KF+H20. 

Sol.  in  H2O  with  decomp. 

Sol.  in  HF  or  HC1  +Aq.  (Mauro  and  Pana- 
bianco,  Gazz.  ch.  it.  12. 80.) 

3MoOF3,  5KF+H2O.  Sol.  in  H2O  with 
decomp.  (Mauro,  Gazz.  ch.  it.  19.  179.) 

Thallous    fluoxyhypomolybdate,    2T1F, 

MoOF3. 
(Mauro,  B.  1894,  27R.  109.) 

Zinc  fluoxyhypomolybdate.  ZnF2,  MoOF3+ 

6H20. 

Rapidly    deliquescent.      Sol.    in    H2O. 
(Mauro,  Real.  Ac.  Line.  1892.  1.  194.) 

Fluoxyhypovanadic  acid. 
See  Fluoxyvanadic  acid. 

Fluoxymanganic  acid. 

Ammonium  fluoxymanganate,  (NH4)2MnOF4. 
Precipitate.    (Nickles.) 

Potassium  fluoxymanganate,  K2MnOF4. 
Precipitate.    (Nickles,  C.  R.  65.  107.) 

/Sesgm'fluoxymanganic  acid. 

Potassium    sesgwifluoxymanganate, 

K4Mn2OF8  =  4KF,  Mn2OF4. 
Precipitate.    (Nickles.) 

Fluoxymolybdic  acid. 

See  also  Fluoxyhypomolybdic,  and  fluoxy- 
permolybdic  acids. 

Ammonium  fluoxymolybdate,  NH4F, 
MoO2F2. 

Sol.  in  H2O.  (Mauro,  Gazz.  ch.  it.  20. 
109.) 

+H2O.  '  More  sol.  in  H2O  than  2NH4F, 
MoO2F2.  (Delafontaine,  N.  Arch.  Sci.  ph. 
nat.  30.  250.) 

Correct  formula  is  3NH4F,  MoO2F2. 
(Mauro,  Gazz.  ch.  it.  18.  120.) 

2NH4F,  MoO2F2.  Much  more  sol.  than 
2KF,  MoO2F2.  (Delafontaine.) 

3NH4F,  MoO2F2.    Sol.  in  H2O.    (Mauro.) 

5NH4F  3MoO2F2+H2O.  Sol.  in  H2O. 
(Mauro,  Gazz.  ch.  it.  20. 109.) 

Ammonium  fluoxymolybdate  molybdate, 

Mo02F2,  4NH4F,  (NH4)2MoO4. 
Sol.  in  H2O,  but  with  decomp.     (Mauro, 
Gazz.  ch.  it.  18. 120.) 

Cadmium  fluoxymolybdate,  CdF2,  Mo02F2-f 

6H2O. 

SI.  efflorescent.  (Delafontaine,  J.  B.  1867. 
236.) 


Cobaltous  fluoxymolybdate,  CoF2,  MoO2F2  + 

6H2O. 

Sol.  in  H2O.  (Delafontaine,  J.  B.  1867. 
236.) 

Cupric    fluoxymolybdate,    CuF2,    MoO2F2  + 

4H2O. 

Deliquescent.  (Mauro,  Real.  Ac.  Line. 
1892, 1. 194. 

Nickel    fluoxymolybdate,    NiF2,    Mo02F2+ 

6H20. 

Sol.  in  H2O.  (Delafontaine,  J.  B.  1867. 
236.) 

Potassium  fluoxymolybdate,  2KF,  MoO2F2  + 
H2O. 

Easily  sol.  in  boiling  H2O. 

Sol.  in  H2O  with  decomp.  Sol.  in  HF. 
(Marchetti,  Z.  anorg.  1895,  10.  68.) 

KF,  MoO2F2+H2O.  Gradually  efflores- 
cent. (Delafontaine.) 

Rubidium  fluoxymolybdate,  2RbF,  2Mo02F2 

+2H20. 

Sol.  in  cold,  more  sol.  in  hot  H2O.  (Dela- 
fontaine.) 

Sodium  fluoxymolybdate,   NaF,    MoO2F2  + 

^H20. 
Sol.  in  H20.    (Delafontaine.) 

Thallous  fluoxymolybdate,  2T1F,  MoO2F2-h 

H2O. 
Sol.  in  hot  H2O.    (Delafontaine.) 

Zinc  fluoxymolybdate,  ZnF2,  MoO2F2+6H20. 
Sol.  in  H20.    (Delafontaine.) 

Fluoxypercolumbic  acid. 

Potassium  fluoxypercolumbate,  2KF,  CbO2F2 
+H2O. 

(Piccini,  Z.  anorg.  2.  21.) 

Sol.  in  H2O  with  decomp. 

Sol.  in  HF.  (Marchetti,  Z.  anorg.  1895, 
10.  67.) 

Fluoxypermolybdic  acid. 

Ammonium    fluoxypermolybdate,     MoO3F2, 

3NH4F. 
Sol.  in  H2O.  '(Piccini,  Z.  anorg.  1.  51.) 

Caesium  fluoxypermolybdate,  Mo03F2,  2CsF 
+H2O. 

(Piccini.) 

Potassium    fluoxypermolybdate,    MoO3F2, 

2KF+H20. 

Not  very  sol.  in  H2O;  more  sol.  in  HF-f- 
A.q  without  decomp.  (Piccini.) 


FLUOXYTUNGSTATE,  ZINC 


355 


Rubidium    fluoxypermolybdate,     MoO3F2, 

2RbF+H2O. 

Somewhat  more  sol.  in  H2O  than  K  salt. 
Easily  sol.  in  HF+Aq.  (Piccini.) 

Fluoxypertantalic  acid. 

Potassium  fluoxypertantalate,  2KF,  TaO2F3 

+H20. 
Sol.  in  H2O.     (Piccini,  Z.  anorg.  2.  21.) 

Fluoxypertitanic  acid,  TiO2F2,  HF. 

Known  only  in  solution.  (Piccini,  B.  18. 
255  R.) 

Ammonium    fluoxypertitanate,    TiO2F2, 
2NH4F. 

Very  unstable.  (Piccini,  Gazz.  ch.  it.  17. 
479.) 

TiO2F2,  3NH4F.    Sol.  in  H2O. 

Sol.  in  H2O2.  (Piccini,  Z.  anorg.  1895,  10 
439.) 

2Ti02F2,  3NH4F.  Sol.  in  H2O.  (Piccini, 
B.  18.  698  R.) 

Barium    fluoxypertitanate,     TiO2F2,     BaF2. 

Precipitate.  Easily  sol.  in  acids.  (Piccini, 
B.  18.  698  R.) 

2TiO2F2,  3BaF2.  Insol.  in  H2O;  sol.  in  dil. 
acids.  (Piccini,  Gazz.  ch.  it.  17.  479.) 

Potassium  fluoxypertitanate,  TiO2F2,   2KF. 
Sol.  in  H2O.    (Piccini,  B.  21.  1391.) 
Sol.  in  H2O2.    (Piccini,  Z.  anorg.  1895,  10. 

438.) 

Fluoxypertungstic  acid. 

Potassium  fluoxypertungstate,  2KF,  WO3F-f- 

H2O. 
(Piccini,  Z.  anorg.  2.  11.) 

Fluoxytantalic  acid. 
See  also  Fluoxypertantalic  acid. 

Ammonium  fluoxytantalate,'3NH4F,  TaOF2. 
Easily  sol.  in  H2O.    The  solution  clouds  up 
by  standing  or  on  warming.    (Joly,  C.  R.  81. 
1266.) 

Fluoxytitanic  acid. 

See  also  Fluoxypertitanic  acid. 

Barium  fluoxytitanate,  TiOF2,  BaF2. 

Insol.  in  H20;  sol.  in  dil.  acids.  (Piccini, 
Gazz.  ch.  it.  17. 479.) 

Fluoxytungstic  acid. 

Ammonium  fluoxytungstate,  2NH4F,  WO2F2. 
Very  sol.  in  H2O.    (Marignac,  A.  ch.  (3)  69. 
65.) 


NH4F,  WO2F2+H2O.  Decomp.  by  H2O. 
Crystallises  unchanged  from  H2O  containing 
HF.  (Marignac.) 

Ammonium    fluoxytungstate    tungstate, 

4NH4F,  WO2F2,  (NH4)2WO4. 
Incompletely  sol.  in  H2O.     Residue  dis- 
solves in  NH4OH+Aq.    (Marignac.) 

Cadmium  fluoxytungstate. 
Very  sol.  in  H2O.    (Marignac.) 

Cupric  fluoxytungstate,  CuF2,  WO2F2+4H2O. 
Very  sol.  in  H2O.    (Marignac,  C.  R.  56.  888. 

Cupric  fluoxytungstate  ammonium  fluoride, 

CuF2,  WO2F2,  NH4F+4H2O. 
Sol.  in  H20.    (Marignac.) 

Manganese  fluoxytungstate. 
Very  sol.  in  H2O.    (Marignac.) 

Nickel    fluoxytungstate,    NiF2,    WO2F2  + 

10H20. 

Deliquescent.  Very  sol.  in  H2O.  (Marig- 
nac.) 

Potassium   fluoxytungstate,    KF,    W02F2  + 

H20: 

Can  be  recrystallised  without  decomp.  only 
from  H2O  containing  HF.  (Marignac,  A.  ch. 
(3)  69.  70.) 

2KF,  WO2F2+H20.  Difficultly  sol.  in 
cold,  more  easily  in  hot  H2O.  (Berzelius.) 

Sol.  in  17  pts.  H2O  at  15°.     (Marignac.) 

Can  be  recrystallised  without  decomp. 
from  H2O,  or  H2O  containing  HF.  (Marig- 
nac.) 

Sol.  in  H2O  with  decomp.     Sol.  in  HF. 
(Marchetti,  Z.  anorg.  1895,  10.  71.) 
'  See  also  Fluoxypertungstate,  potassium. 

Silver  fluoxytungstate. 
Very  easily  sol.  in  H2O.    (Marignac.) 

Sodium  fluoxytungstate,  2NaF,  WO2F2. 

More  sol.  in  H2O  than  the  corresponding  K 
compound.  (Berzelius.) 

Thallous  fluoxytungstate,  T1F,  W02F2. 

Insol.   in   H2O.      Decomp.    by   H2O. 
(Ephraim  and  Heymann,  B.  1909,  42.  4463.) 

2T1F,  WO2F2.  Insol.  in  H2O'but  decomp. 
thereby.  (Ephraim  and  Heymann,  B.  1909, 
42.  4462.) 

3T1F,  2WO2F2.  Insol.  in  H2O.  Decomp. 
by  acids.  (Ephraim  and  Heymann,  B.  1909, 
42.  4462.) 

Zinc  fluoxytungstate,  ZnF2,  WO2F2+10H2O. 
Very  sol.  in  H2O.    (Marignac.) 


356 


FLUOXYURANIC  ACID 


Fluoxyuranic  acid. 

Ammonium  fluoxyuranate,  3NH4F,  UO2F2. 

Easily  sol.  in  H2O,  less  in  HF.  Insol.  in 
alcohol.  (Bolton.) 

100  g.  solution  sat.  at  27°  contain  10.11  g. 
salt. 

100  g.  solution  sat.  at  81.3°  contain  20.71  g. 
salt. 

(Burger,  Dissert.  1904.) 

Barium    fluoxyuranate,    3BaF2,    2U02F2+ 

2H2O. 

Traces  dissolve  in  hot  H2O.  Easily  sol.  in 
dil.  acids.  (Bolton.) 

Potassium  fluoxyuranate,  3KF,  ITO2F2. 

Sol.  in  8  pts.  H20  at  21°.  Insol.  in  alcohol 
and  ether.  (Bolton,  J.  pr.  99.  269.) 

Does  not  exist.  (Smithells,  Chem.  Soc.  43. 
125.) 

4KF,  UO2F2.  Insol.  in  H2O.  Easily  sol.  in 
dil.  acids.  (Ditte,  C.  R.  91.  115.) 

5KF,  2UO2F2.  (Baker,  Chem.  Soc.  35. 
760.) 

3KF,  2UO2F2+2H2O.    (Baker.) 

Sodium  fluoxyuranate,  NaF,  U02F2. 

+2H2O.    Not  efflorescent. 

+4H20.  Insol.  in  H2O  and  dil.  acids.  SI. 
sol.  in  cone.  HCl+Aq.  Sol.  in  cone.  H2SO4. 
(Bolton,  J.  B.  1866. 212.) 

4NaF,  U02F?.     (Ditte.) 

Does  not  exist.  (Smithells,  Chem.  Soc. 
43.  125.) 

Fluoxyvanadic  acid. 

Ammonium  fluoxyvanadate,  12NH4F,  V2O6, 
2VOF3. 

Easily  sol.  in  H20,  and  not  attacked  by 
cold  cone.  H2SO4.  (Baker,  Chem.  Soc.  33, 
388.) 

Formula  is  3NH4F,  VO2F.  (Petersen,  J 
pr.  (2)  40.  289.) 

3NH4F,  VO2F.  Sol.  in  H20.  (Petersen 
U.) 

Much  less  sol.  in  H20  in  presence  of  NH4F 
(Piccini  and  Giorgis,  Gazz.  ch.  it.  27. 1.  65.). 

+H2O.  (Piccini  and  Giorgis,  Gazz.  ch.  it 
1892,  22.  55.) 

3NH4F,  VOF2.  "Hypoyanadate."  Quite 
sol.  in  H2O.  Very  si.  sol.  in  MF+Aq.  Less 
sol.  in  alcohol  than  in  H2O.  (Petersen,  J 
pr.  (2)  40.  195.) 

2NH4F,  VOF2.    Sol.  in  H2O.     (Petersen.; 

+H20.    (Piccini  and  Giorgis.) 

7NH4F,  4VOF2+5H2O.  Very  sol.  in  H2O 
(Petersen.) 

3NH4F,  2VO2F.  Sol.  in  H2O  without  de- 
comp.  Sol.  in  cone.  HF+Aq.  (Piccini  anc 
Giorgis,  Gazz.  ch.  it.  24.  1.  68.) 

3NH4F,  2VOF3+H2O.  Sol.  in  H2O  with 
decomp. 

V2O5,  2NH4F.    (Ditte,  C.  R.  106.  270.) 


V2O6,  8NH4F+4H2O.    As  above. 
V206,  4NH4F+4H20.    As  above.    Sol.  in 
H20. 

Ammonium      hydrogen      flucfo'oxyvanadate, 

7NH4F,  HF,  4VO2F. 
Very  sol.  hi  H2O.    (Petersen,  J.  pr.  (2)  40. 

284.)  . 

Ammonium    hydrogen     fnfluoxyvanadate, 

3HF,  9NH4F,  5VOF3. 
Easily  sol.  in  H2O.    SI.  sol.  in  MF+Aq. 
Petersen,  J.  pr.  (2)  40. 280.) 

3NH4F,    3HF,   2VOF3.     Sol.   in   H2O. 
(Baker,  Chem.  Soc.  33.  388.) 

Identical  with  3HF,   9NH4F,   5VOF3. 
Petersen.) 

Barium  fluoxyvanadate,  BaF2,  VO2F. 

Ppt.     (Ephraim,  Z.  anorg.  1903,  35.  79.) 

Cadmium    fluoxyvanadate,    CdF2,    VOF2  + 
7H2O. 

Hypovanadate."    As  the  Co  salt.    (Pic- 
cini and  Giorgis.) 

Cobalt  fluoxyvanadate,  CoF2,  VOF2+7H2O. 
"  Hypovanadate."     Sol.  in  H2O.     (Piccini 
and  Giorgis.) 

Nickel  fluoxyvanadate,  NiF2,  VOF2+7H2O. 

"Hypovanadate."  As  the  Co  salt.  (Piccini 
and  Giorgis.) 

Potassium  fluoxyvanadate,  7KF,  3VOF2. 

Very  si.  sol.  in  H2O  and  MF+Aq.  Easily 
sol.  in  dil.  acids.  (Petersen,  J.  pr.  (2)  40. 
199.) 

2KF,  VOF2.   As  above.    (Petersen.) 

2KF,  2V2O5+8H2O.  Sol.  in  H2O  and 
H2SO4.  (Ditte,  C.  R.  105.  1067.) 

2KF,  3V2O6+5H2O.    As  above. 

2KF,  4V2O6+8H2O.    As  above. 

4KF,  V2O5.     Less  sol.  than  4KF,  3V205. 

+2H2O,  and  +3H2O.    Sol.  in  H2O. 

4KF,  3V2O6+4H2O,  and  +6H2O.  Less 
sol.  than  2KF,  3V2O6+5H2O. 

8KF,  V2O5+2H2O,  and  +3H2O.  Sol.  in 
H2O. 

Potassium   fn'fluoxyvanadate,    2KF,    VOF3. 

Ppt.    (Petersen,  J.  pr.  (2)  40.  272.) 

6KF;  V206,  2VOF3+2H2O.  Sol.  in  H20. 
Insol.  in  cold  cone.  H2SO4.  (Baker,  Chem. 
Soc.  33.  300.) 

Formula  is  3KF,  2V02F.  (Piccini  and 
Giorgis.) 

See  also  Fluovanadate  fluoxyvanadate, 
potassium. 

Potassium  flucftoxyvanadate,  2KF,  VO2F. 

Easily  sol.  in  H2O.  (Petersen,  J.  pr.  (2)  40. 
278.) 


FULMINATING  PLATINUM 


357 


3KF,  VO2F.     As  above.     (Petersen.) 
3KF,  2VO2F.     Sol.  in  H2O;  scarcely  at- 
tacked by  H2SO4.     (Piccini  and  Giorgis.) 

Potassium  hydrogen  fluoxyvanadate,   3KF, 

HF,2VOF3. 
Sol.  in  H20.    (Petersen.) 

Sodium  fluoxyvanadate,  8NaF,  3VOF2-f 
2H20. 

Sol.  in  HoO.    (Petersen,  J.  pr.  (2)  40.  200.) 

3NaF,  V02F,  VOF3  (?).  Very  easily  de- 
comp.  (Piccini  and  Giorgis.) 

2NaF,  2V2O6-hlOH2O.  Sol.  in  H2O. 
(Ditte,  C.  R.  106.  270.) 

4NaF,  V2O6.    As  above. 

4NaF,  3V2O6+18H2O.    As  above. 

6NaF,  V2O6+5H2O.    As  above. 

8NaF,  V206-f  3H2O.     (As  above. 

Thallous  fluoxyvanadate,  2T1F,  VOF2. 

Somewhat  sol.  in  cold  H2O  without  decomp. 

Sol.  in  boiling  H2O  with  exception  of  a 
black  residue,  which  is  easily  sol.  in  dil. 
H2SO4.  (Ephraim,  B.  1909,  42.  4460.) 

3T1F,2VO2F.  Insol.inH2O.  Sol.  in  H20 
containing  H2SO4.  (Ephraim  and  Hey- 
mann,  B.  1909,  42.  4459.) 

Zinc  fluoxyvanadate,  ZnF2,  ZnO,  2VOF8  + 
14H2O. 

Decomp.  on  air;  sol.  in  H2O.  (Baker, 
Chem.  Soc.  33.  388.) 

True  composition  is  represented  by  the  for- 
mula ZnF2,  VO2F+7H2O.  (Petersen.) 

ZnF2,  VO2F+7H2O.  Very  sol.  in  H2O. 
(Piccini  and  Giorgis.) 

ZnF2,  VOF2+7H2O.  "Hypovanadate." 
Sol.  in  cold  H2O,  but  decomp.  by  boiling; 
sol.  in  dil.  HF+Aq.  (Piccini  and  Giorgis.) 

Fluozirconic  acid. 

Ammonium  fluozirconate,  (NH4)2ZrF6. 
Sol.  in  H2O. 
3NH4F,  ZrF4.    Sol.  in  H2O.     (Marignac.) 

Cadmium  fluozirconate,  2CdF2,  ZrF4+6H2O. 

Sol.  in  H2O;  can  be  recrystalised  therefrom. 
(Marignac,  A.  ch.  (3)  60.  257.) 

CdZrF6+6H2O.    Sol.  in  H2O.    (Marignac.) 

Caesium  fluozirconate,  CsF,  ZrF4+H2O. 

Sol.  in  H2O  without  decomp.  (Wells, 
Z.  anorg.  1895,  10.  434.) 

2CsF,  ZrF4.  Sol.  in  H20  without  decomp. 
(Wells,  Z.  anorg.  1895,  10,  434.) 

2CsF,  3ZrF4+2H2O.  Only  si.  sol.  in  H20. 
(Wells,  Z.  anorg.  1895,  10.  434.) 

Cupric  fluozirconate,  2CuF2,  ZrF4-f-12H2O. 

Easily  sol.  in  cold  H2O.  (Marignac,  A.  ch. 
(3)  60.  296.) 

3CuF2,  2ZrF4  +  16H2O.  Sol.  in  H2O. 
(Marignac.) 


Lithium  fluozirconate,  2LiF,  ZrF4. 

Ppt.     (Wells,   Am.   J.   Sci.   1897,    (4)   3. 

4LiF,  ZrF4  +  3^H2O.  Sol.  in  H2O  with 
decomp.  (Wells,  Am.  J.  Sci.  1897,  (4)  3. 
469.) 

Magnesium  fluozirconate,  MgZrF6+5H20. 
Sol.  in  H2O.     (Marignac.) 

Manganous  fluozirconate,  MnZrF6+5H2O. 
Sol.  in  H2O.    (Marignac,  J.  pr.  83.  202.) 

Nickel  fluozirconate,  2NiF2,  ZrF4+12H20. 

Sol.  in  H2O.  (Marignac,  A.  ch.  (3)  60. 
291.) 

NiZrF6+6H2O.  Sol.  in  H2O.  (Marig- 
nac.) 

Nickel  potassium  fluozirconate,  K2ZrF6, 

NiZrF6+8H2O. 
Sol.  inH20.    (Marignac.) 

Potassium  fluozirconate,  KF,  ZrF4+H20. 

Much  more  sol.  in  hot,  than  cold  H2O. 
(Marignac.) 

2KF,  ZrF4  =  K2ZrF6.  100  pts.  H20  dis- 
solve at  2°,  0.781  pt.;  at  15°,  1.41  pts.;  at  19.° 
1.69  pts.;  at  100°,  25.0  pts.  K2ZrF6.  (Marig- 
nac.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  829.) 

3KF,  ZrF4. 

Sodium  fluozirconate,  5NaF,  ZrF4. 

100  pts.  H20  dissolve  0.387  pt.  at  18°,  and 
1.67  pts.  at  100°.  (Marignac.) 

2NaF,  ZrF4.  (Wells,  Am.  J.  Sci.  1897,  (4) 
3.  469.) 

5NaF,  2ZrF4.  Sol.  in  H2O  with  decomp. 
(Wells.) 

Tellurium  fluozirconate,  TeF,  ZrF4. 

Sol.  in  H2O  without  decomp.  (Wells, 
Am.  J.  Sci.  1897,  (4)  3.  470.) 

+H2O.  Sol.  in  H2O  without  decomp. 
(Wells.) 

3TeF,  ZrF4.  Sol.  in  H2O  without  decomp. 
(Wells.) 

5TeF,  3ZrF4.  Sol.  in  H2O  without  decomp. 
(Wells.) 

Zinc  fluozirconate,  ZnZrF6+6H20. 

Sol.  inH2O.    (Marignac.) 

2ZnF2,  ZrF4+12H2O.  Sol.  in  H2O.  (Mar- 
ignac, A.  ch.  (3)  60.  257.) 

Fulminating  gold. 
See  Auroamidoimide. 

Fulminating  platinum. 
See  Fulminoplatinum. 


358 


FULMINATING  SILVER 


Fulminating  silver. 
See  Silver  nitride. 

Fulminoplatinum  compounds. 
See— 

Dichlorofulminoplatinum. 
TVicUorofulmmoplatinum. 
Te^achlorofulminoplatinum. 
Chloroxyfulminoplatinum. 

Fuscocobaltic  chloride,  Co(NH3)4(OH)Cl2 

+H20. 

Sol.  in  H2O,  from  which  it  is  precipitated 
by  NH4Cl+Aq;  decomp.  by  boiling  H2O; 
pptd.  from  aqueous  solution  by  alcohol. 
(Fremy,  C.  R.  32.  501.) 

—  nitrate,  Co(NH3)4(OH)(NO3)2+H2O. 
Sol.  in  H2O.     Properties  as  the  chloride. 
(Fremy.) 

sulphate,   Co(NH3)4(OH)SO4+l^H2O. 

Sol.  in  H2O.  Insol.  in  NH4OH+Aq. 
(Fremy,  C.R.  32.  501.) 

Insol.  in  H2O.  Sol.  in  cone.  HCl+Aq,  or 
H2SO4,  from  which  it  is  precipitated  by  H2O. 
(Vortmann,  N.  6.  412.) 

Fusible  white  precipitate. 

See  Mercuricfo'ammonium  chloride. 

Gadolinium,  Gd. 

(Marignac,  C.  R.  102.  92.) 

Gadolinium  bromide,   GdBr3+6H2O. 

Sol.  in  HBr.  (Benedicks,  Z.  anorg.  1900, 
22.  403.) 

Gadolinium    chloride,    GdCl3+6H2O. 

Somewhat  deliquescent.  Sol.  in  H2O. 
(Benedicks.) 

Gadolinium  platinum  chloride. 
See  Chloroplatinate,  gadolinium. 

Gadolinium  fluoride,  GdF3. 

Insol.  in  H2O ;  si.  sol.  in  hot  HF.  (Popovici, 
B.  1908,  41.  635.) 

Gadolinium  hydroxide,  Gd(OH)8. 

Ppt.    (Benedicks,  Z.  anorg.  1900,  22.  402.) 

Gadolinium  oxide,  Gd2O3. 

Sol.  in  acids,  (de  Boisbaudran,  C.  R.  111. 
394.) 

Somewhat  hydroscopic;  easily  sol.  in  acids. 
(Benedicks.) 

Gallium,  Ga. 

Not  decomp.  by  H2O;  easily  sol.  in  cold 
HC1  +Aq.  Slowly  sol.  in  warm  dil.  HNO3+ 
Aq.  Not  attacked  by  cone.  HNO3  free  from 


N2O3    below    40-50°,    and    only    slowly    in 
presence  of  N2O3.    (Dupre,  C.  R.  86.  720.) 

Easily  sol.  in  cold  or  warm  KOH+Aq. 
(de  Boisbaudran,  A.  ch.  (5)  10.  100.) 

Gallium  bromide,  GaBr3. 

Deliquescent,  and  sol.  in  H2O. 

Gallium  bichloride,  GaCl2. 

Deliquescent,  and  decomp.  by  H20.  (Nil- 
son  and  Petersen,  C.  R.  107.  527.) 

Gallium  chloride,  GaCl3. 

Deliquescent,  and  very  sol.  in  little  H2O. 
Decomp.  by  much  H2O,  with  formation  of 
basic  salt,  which  is  slowly  sol.  in  dil.  HC1 
+Aq. 

Gallium  hydroxide. 

Sol.  in  acids;  sol.  in  KOH  or  NaOH+Aq, 
less  easily  in  NH4OH+Aq,  even  in  presence 
of  ammonium  salts. 

Gallium  iodide,  GaI3. 

Deliquescent,  and  sol.  in  H2O.  (de  Bois- 
baudran and  Jungfleisch,  C.  R.  86.  578.) 

Gallium  sw&oxide,  GaO  (?). 
Sol.  in  HNO3+Aq.    (Dupre.) 
Sol.  in  dil.  H2SO4+Aq. 

Gallium  oxide,  Ga2O3. 
Sol.  in  acids. 

Germanium,  Ge. 

Insol.  in  HCl+Aq.  Easily  sol.  in  aqua 
regia.  Decomp.  by  HNO3+Aq  to  oxide. 
Cone.  H2SO4  decomp.  to  sulphate.  Insol.  in 
boiling  KOH+Aq.  (Winkler,  J.  pr.  (2)  34. 
177;  36. 177.) 

Germanium  te^rabromide,  GeBr4. 
Decomp.  by  H3O.     (Winkler.) 

Germanium  bichloride,  GeCl2. 
Decompl  by  H2O.    (Winkler.) 

Germanium  t eti  ochloride,  GeCl4. 

Sinks  in  H2O,  and  is  gradually  decomp. 
thereby.  (Winkler,  J.  pr.  34.  177.) 

Insol.  in  and  not  attacked  by  hot  cone. 
H2S04.  (Friedrich,  W.  A.  B.  102,  2b.  540.) 

Germanium  chloroform,  GeHCl3. 

Decomp.  by  H2O.  Sol.  in  HCl+Aq. 
(Winkler.) 

Germanium  teti  afluoride,  GeF4. 

Deliquescent,  and  sol.  in  H2O. 

+3H2O.  Deliquescent.  Melts  in  its 
crystal  H2O  when  warmed.  (Winkler.) 


GLASS 


359 


Germanium  potassium  fluoride. 
See  Fluogermanate,  potassium. 

Germanium  hydride,  GeH4. 

SI.  sol.  in  hot  HC1.  Sol.  in  NaOCl+Aq. 
(Voegelen,  Z.  anorg.  1902,  30.  327.) 

Germanium  te^raiodide,  Gel4. 

Deliquescent,  and  sol.  in  H2O  with  decomp. 
(Winkler.) 

Germanium  wowoxide,  GeO. 

Not  appreciably  sol.  in  dil.  H2SO4+Aq. 
Easily  sol.  in  HCl+Aq.  Insol.  in  alkalies. 
(Winkler,  J.  pr.  (2)  34.  177.) 

Somewhat  sol.  in  H2O ;  insol.  in  H2SO4-f  Aq, 
even  when  hot  and  cone,  (van  Bemmelen,  R. 
t.  c.  6.  205.) 

Germanium  dioxide,  GeO2. 

Not  very  difficultly  sol.  in  H2O. 

Sol.  in  247.1  pts.  H2O  at  20°;  in  93.3  pts. 
at  100°.  (Winkler.) 

Easily  sol.  in  alkali  carbonates  or  hydrates 
+Aq;  si.  sol.  in  acids. 

Germanium  oxychloride,  GeOCl2. 

Insol.  in  H2O:  sol.  in  acids.  (Winkler,  J. 
pr.  (2)  36. 177.) 

Germanium  mowosulphide,  GeS. 

Sol.  in  402.9  pts.  H2O.  Sol.  in  cone,  hot 
HCl+Aq.  Sol.  in  KOH+Aq.  Sol.  in 
(NH4)2S+Aq  when  precipitated.  Insol.  in 
(NH4)2S+Aq  if  crystalline.  Also  exists  in  a 
colloidal  state.  (Winkler.) 

Germanium  ^'sulphide,  GeS2. 

Sol.  in  221.9  pts.  H2O.  Easily  sol.  in. 
KOH+Aq,  or  NH4OH+Aq.  Insol.  in  acids. 
Exists  also  in  a  colloidal  state.  (Winkler.) 

Glass. 

Numerous  and  extensive  researches  have 
been  made  on  the  action  of  H2O  and  various 
solutions  on  glass.  The  older  work  has  a  cer- 
tain historical  interest,  but  only  a  brief  state- 
ment of  some  of  the  more  important  results 
can  be  given  here.  For  a  very  thorough 
resume  of  the  work  before  the  year  1861, 
Storer's  Dictionary,  p.  555,  should  be  con- 
sulted. 

All  glass  is  more  or  less  attacked  by  H2O, 
the  more  easily  the  greater  the  amount  of 
alkali  present,  the  finer  it  is  powdered,  and 
the  higher  the  temperature. 

Glass,  as  that  of  a  flask,  is  decomposed  to  a  consider- 
able exlent  by  several  days'  boiling  with  H2O,  a  portion 
of  the  fixed  alkali  being  dissolved,  but  when  powdered 
glass  is  rubbed  with  distilled  H2O  in  a  mortar,  the  H2O 
remains  pure  and  exhibits  no  alkalinity.  (Scheele.) 

Glass  of  alembics  is  partially  dissolved  by  long  boil- 
ing with  H2O.  (Lavoiser.) 

H  2O  extracts  potash  or  soda  from  glass  together  with 


Powdered  lead  glass  gives  up  appreciable  amounts  of 
)O  to  weakly  acidified  H2O.     (Pelouze.) 


a  portion  of  the  silica,  the  decomposition  taking  place 
the  more  easily  in  proportion  as  the  glass  is  richer  in 
alkalies,  more  minutely  divided,  or  the  temperature  of 
the  water  higher.  (Bischof,  Kastn.  Arch.  1.  443.) 

Powdered  crown  glass  and  some  varieties  of  window 
glass  render  cold  H2O  alkaline  when  in  contact  there- 
with. (Dumas.) 

100  pts.  finely  divided  flint  glass  lose  7  pts.  potash 
when  boiled  one  week  with  H2O.  (Griffiths,  Q.  J.  Sci. 
20.  258.) 

Retorts  of  ordinary  or  flint  glass  are  partially  dis- 
solved by  H2O  when  it  is  evaporated  therein.  (Chev- 
reul,  1811.) 

Finely  powdered  plate-glass  (Faraday,  Pogg.  18.  569), 
and  Thuringian  potash  glass  (Ludwig,  Arch.  Pharm.  91. 
47)  redden  moistened  turmeric  paper. 

The  alkaline  reaction  disappears  by  continued  wash- 
ing, but  reappears  when  the  glass  is  freshly  rubbed. 
(Griffiths.) 

Cold  HzO  takes  up  SiO2  as  well  as  alkali  from  glass 
powder.  (Fuchs.) 

PbO 

When  powdered  white  glass,  containing  12.4%  Na2O, 
15.5%  CaO,  and  72.1%  SiO2,  is  treated  repeatedly  with 
HjO,  more  than  3%  of  the  glass  is  dissolved,  and  the 
undissolved  part  gives  up  1.5%  CaO  to  HCl+Aq  with 
effervescence.  A  glass  containing  more  alkali,  i.  e. 
16.3%  Na2O,  6.4%  CaO,  77.3%  SiO2,  lost  with  the  same 
treatment  18.2%,  and  the  residue  gave  up  2%  CaO  to 
HCl+Aq.  (Pelouze,  C.  R.  43.  117.) 

In  the  above  case  the  fineness  of  the  glass  has  an 
influence  as  well  as  its  composition.  When  the  same 
sample  of  glass  was  boiled  1  hour  with  HsO,  amounts 
were  dissolved  in  the  proportion  1  :  4  :  28,  according  as 
the  glass  was  in  form  of  a  coarse,  fine,  or  very  fine 
powder.  Glass  of  the  composition  of  the  above  samples, 
as  given  by  Pelouze,  lost  10  and  32%  respectively. 

If  powdered  glass  is  boiled  with  H2O  and  CO2  con- 
ducted into  the  solution,  it  is  absorbed;  if  boiled  with 
K2SO4.  Na2SO4  is  dissolved.  (Pelouze.) 

Glass  tubes  are  converted  into  a  white  crystalline 
mass  by  heating  with  H2O  several  months  to  75-150°; 
lead  glass  and  Bohemian  glass  most  easily,  English 
crown  glass  least.  A  little  H2O  attacks  glass  more 
than  much  H2O. 

The  action  of  H2O  is  greatly  increased  by 
finely  pulverising  the  glass. 

H2O  dissolved  10%  of  a  glass  containing 
12%  Na20,  15.5%  CaO,  and  72.5%  SiO2,  and 
32%  of  another  glass  containing  16.3%  Na2O, 
6.4%  CaO,  and  77.3%  SiO2.  (Vogel,  B.  A. 
Munchen,  1867.  437.) 

Action  of  H2O  on  a  glass  containing  74% 
Si02,  8.6%  CaO,  14%  Na2O  0.6%  K2O,  with 
traces  of  A12O3,  Fe2O3,  MnO,  and  MgO. 

By  boiling  with  H20  a  decrease  of  3.9  mg. 
was  observed  for  the  first  hour,  which  soon 
became  constant  at  2.2  mg.  per  hour.  The 
action  was  then  proportional  to  the  time,  and 
also  to  the  surface  in  contact  with  the  liquid, 
but  independent  of  the  amount  of  liquid 
evaporating. 

The  action  decreases  rapidly  with  the  tem- 
perature, so  that  at  90-100°  only  ^  as  much 

ass  is  dissolved  as  by  boiling  H2O .  (Emmer- 
ag,  A.  150.  257.) 

When  steam  condenses  in  tubes  of  Na  glass, 
they  are  so  strongly  attacked  that  the  H2O 
has  an  alkaline  reaction,  but  tubes  of  hard  or 
Bohemian  K  glass  are  not  so  strongly  at- 
tacked. (Tollens,  B.  9.  1540.) 

The  effect  of  H2O  is  so  great  as  to  impart  a 
distinctly  alkaline  reaction  to  water  condens- 
ing in  a  tube  of  ordinary"glass.  By  condensing 
water  in  long  tubes  of  various  kinds  of  glass 
the  following  results  were  obtained. 


360 


GLASS 


I.  Easily  fusible  Thuringian  glass.     Sur- 
face exposed  =  324  sq.  cm. 

After  2  hours,  62.0  mg.  KOH  were  dis- 
solved. 

After  3  hours  more,  36.0  mg.  KOH  were  dis- 
solved. 

After  3  hours  more,  33.2  mg.  KOH  were  dis- 
solved. 

After  3  hours  more,  20.8  mg.  KOH  were  dis- 
solved. 

After  3  hours  more,  20.8  mg.  KOH  were  dis- 
solved. 

Or,  in  14  hours,  172.8  mg.  KOH  were  dis- 
solved. 

II.  Less  easily  fusible  Thuringian  glass. 
Surface  exposed  =  499  sq.  cm. 

After  3  hours,  19.2  mg.  KOH  were  dis- 
solved. 

After  3  hours  more,  15.2  mg.  KOH  were  dis- 
solved. 

After  3  hours  more,  12.4  mg.  KOH  were  dis- 
solved. 

After  3  hours  more,  11.2  mg.  KOH  were  dis- 
solved. 

Or,  after  12  hours,  58.0  mg.  KOH  were  dis- 
solved. 

III.  Combustion  tubing  of  very  difficultly 
fusible  Bohemian  glass.     Surface  exposed 
1130  sq.  cm. 

After  3  hours  4.16  mg.  KOH  were  dis- 
solved. 

After  3  hours  more  4.16  mg.  KOH  were  dis- 
solved. 

After  3  hours  more  4.16  mg.  KOH  were  dis- 
solved. 

After  3  hours  more  4.16  mg.  KOH  were  dis- 
solved. 

Or,  after  12  hours,  16.64  mg.  KOH  were  dis- 
solved. 

.    IV.  Easily  fusible  Bohemian  glass.     Sur- 
face exposed  =  1394  sq.  cm. 

After  3  hours,  7.88  mg.  KOH  were  dis- 
solved. 

After  3  hours  more,  8.56  mg.  KOH  were  dis- 
solved. 

After  3  hours  more,  1.97  mg.  KOH  were  dis- 
solved. 

Or,  after  9  hours,  24.32  mg.  KOH  were  dis 
solved.  (Kreusler  and  Henzold,  B.  17.  34V 

From  the  above  the  following  table  has 
been  calculated. 

50  ccm.  H2O  dissolves  from  a  surface  o 
1000  sq.  m.  in  1  hour: — 

96.0  mg.  from  easily  fusible  Thuringian 
glass. 

12.8  mg.  from  less  fusible  Thuringian  glass 

1.2  mg.  from  combustion  tube  of  Bohemian 
glass. 

2.0  mg.  from  harder  tube  of  Bohemian 
glass. 

(Kreusler  and  Henzold,  B.  17.  34.) 

100  ccm.  H2O  dissolves  so  much  glass  from 
flask  every  2  seconds,  when  in  contact  there- 
with that  0.1  ccm.  y%  normal  oxalic  acid  i 
neutralised  thereby.     (Bohlig,  Z.  anal.  23 
518.) 


Action  of  H2O  on  various  kinds  of  Na  glass, 
g.  of  finely  powdered  glass  was  boiled  10-15 
minutes  in  a  silver  dish  with  100  ccm.  H2O, 
nd  the  per  cent  of  Na2O  (or  K2O)  in  the 
olution  was  determined. 

%Na20 
(K20) 

)rthoclase  feldspar  .          .     .    .          .     0.17 
lass  of  a  Bohemian  combustion  tube  .     0.56 
flask  (German  manuf.)        .     0.69 
"  champagne  bottle      .          .     1.7 

STatrolite  .  .  .  \  .1.32 
lass  of  a  wine  bottle  (Hungarian)  .  2 . 22 
lass  which  was  attacked  by  H2O 

under  pressure         .          .          .3.7 
l,ead  glass 

Grlass  that  broke  easily      .         .         .4.8 
Glass  tubing  that  became  rough  when 

fused     .         .        V.         .6.1 
lass  tubing  that  became  opaque  by 

fusing  i>.-,'      .          .          .14.35 

Solid  water  glass       .         .         .         .26.97 
(Wartha,  Z.  anal.  24.  220.) 

The  relative  ease  by  which  various  kinds  of 
glass  are  attacked  by  H2O  is  shown  by  the 
Allowing  table.  The  glass  was  powdered  and 
leated  on  a  water  bath  with  exclusion  of 
atmospheric  CO2. 

Potassium  water  glass     »  ;i^J  291 

Sodium  water  glass     .         .-:.,  196 

Yellow  glass  rich  in  alkali  .  34 

Thuringian  glass         .          .  19 

Ditto  from  Tittel  and  Co*.  8 

Window  glass    . 

Lead  glass  from  Jena  6 

Bohemian  glass  from  Kavalier  2 . 4 

Lead  crystal  glass       .          .  1.4 

Thermometer    glass,     16IV,     from 

Jena.          ...  1.0 

Zinc  glass,  362,  from  Jena  .  0.8 

Lead  glass,  434,.  from  Jena  0 . 6 

Lead  glass,  483,  from  Jena  0.2 

Heaviest  lead  silicate,  from  Jena        0 . 0 
(Mylius,  C.  C.  1888.  1313.) 


Solubility  of  various  kinds  of  glass  in  H2O. 

The  amounts  dissolved  from  various  kinds 
of  glass  by  heating  5  hours  with  H2O  were  as 
follows. 
Yellow  glass  rich  in  alkali  (13% 

K2O,  15%  Na2O)          .         .       249  mg. 
Poor  Thuringian  glass  (6.6%  K2O, 

16.5%  Na2O)       .          .          .     91.4     " 
Glass  from  Tittel  and  Co.  (7.1% 

K2O,  14.3%  Na2O)       .         .     30.4     " 
Bottle  glass  from  Schilling  (4.2% 

K2O,  11.9%  Na2O)       .         .     13.0     " 
Bohemian    glass    from    Kavalier 

(13.3%  K2O,  11.4%  Na2O)  .     10.1     " 
Rhenish    window    glass    (13.5% 

Na20)  .          .          .       8.4     " 

Lead  crystal  glass  from  Ehren- 

feld(12.1%K2O)          .          .       8.5     " 
Green  bottle  glass  (1.3%  K2O,  9.5 

%  Na20)    .         .         .         .6.5     " 


GLASS 


361 


Solubility  of  various  kinds  of  glass  in  H2O — 

Continued. 
Thermometer    glass    16III    from 

Jena  (14.0%  Na2O,  7%  ZnO)       6.4  mg 
Lead  glass,  No.  483,  from  Jena 

(47%PbO,7.3%K20).         .       3.3     " 
Lead  silicate       .          .          .  0.6     " 

(Mylius  and  Forster,  B.  22.  1100.) 

By  calculation  from  the  electrical  conduct- 
ivity of  the  solutions  formed,  various  data 
were  obtained  by  Kohlrausch  (B.  24.  3565), 
which  showed  that  different  varieties  of  glass 
were  attacked  in  very  different  degree  by 
cold  H2O,  and,  moreover,  the  amount  dis- 
solved was  proportionately  much  greater 
during  the  first  few  minutes  of  treatment 
with  H2O  than  afterwards,  and,  furthermore, 
the  rate  of  decrease  was  much  faster  for  good 
glass  than  poor.  Increase  of  temperature 
increased  the  rate  of  solubility  to  a  very 
great  degree,  the  increase  for  1°  C.  being 
about  17%.  In  7  hours  at  80°  half  as  much 
was  dissolved  as  in  6  months  at  18°.  Ex- 
tensive tables  are  given.  (Kohlrausch,  B. 
24.  3651.)  See  also  Kohlrausch  (W.  Ann.  44. 
577). 

A  very  extensive  research  on  the  action  of 
H2O  on  glass,  with  a  historical  review  of  the 
work  previously  done  on  the  subject,  has  been 
published  by  Mylius  and  Forster.  (Z.  anal. 
31.  241 .)  The  general  results  may  be  summed 
up  as  follows: — 

1.  The  solution  of  glass  in  H20  is  caused  by 
a   decomposition,    by   which   free   alkali   is 
formed. 

2.  The  silicic  acid  of  the  glass  is  brought 
into  solution  by  a  secondary  reaction  of  the 
free  alkali  in  the  solution. 

3.  The  constituents  of  the  solution  change 
according   to  the   conditions  of   the  diges- 
tion. 

4.  The  amount  of  alkali  going  into  solution 
from  a  given  surface  under  certain  conditions 
is  a  measure  for  the  resistance  of  a  glass  under 
those  conditions. 

5.  The  rate  of  attack  of  glass  surfaces  by 
cold  H2O  decreases  rapidly  with  the  length 
of  time  of  digestion,  and  finally  approaches  a 
constant  value. 

6.  The   solubility   increases   very   rapidly 
with  increase  of  temperature. 

7.  The  ratio  of  the  solubility  of  several 
kinds  of  glass  is  dependent  on  the  tempera- 
ture. 

8.  From  glasses  which  show  the  same  ease 
of  attack  unequal  amounts  of  substance  may 
be  dissolved. 

9.  The  solubility  of  a  glass  is  influenced  by 
the  condition  of  the  surface  from  "weather- 
ing" by  prolonged  exposure  to  the  GO2  and 
H2O  of  the  air. 

•  10.  The  poorer  a  glass  is  the  less  will  its 
solubility  decrease  by  prolonged  treatment 
with  H2O. 

11.  A  good  glass  is  essentially  less  easily 


attacked  after  having  been  previously  treated 
withH2O. 

12.  After  treatment  with  H2O,  glass  sur- 
faces have  the  property  of  fixing  alkali  from 
the  solutions  formed,  and  giving  it  up  again 
by  a  subsequent  treatment  with  H2O. 

13.  Potassium  glass  is  much  more  sol.  than 
sodium    glass     (contrary    to    previous    re- 
searches),  but   the  difference    decreases   as 
the  glass  becomes  richer  in  CaO. 

14.  In  glass  flasks  which  are  to  be  only 
slightly  attacked  by  cold  or  hot  H2O,  the  CaO, 
alkalies,  and  SiO2  must  stand  in  a  fixed  rela- 
tion to  each  other. 

15.  Of  the  more  common  varieties  of  glass, 
lead  flint  glass  is  least  sol.  in  H2O,  but  its 
surface  is  corroded,  and  it  is  easily  decomp. 
by  acids. 

(Mylius  and  Forster,  Z.  anal.  31.  241.) 

Bottle  glass  containing  much  AlzOs  is  easily  attacked 
by  acids. 

From  powdered  flint  glass,  boiling  HC1  +Aq  extracts 
K,  but  no  Pb.  (Griffiths.) 

Bottles  of  flint  glass  with  (NH^COs+Aq  became  so 
fragile  that  on  shaking  pieces  of  glass  were  detached. 
(Griffiths.) 

All  glass  is  decomp.  by  HF. 

Cone.  H3PO4  also  attacks  all  glass. 

Glass  containing  small  amounts  of  SiO2  are  attacked 
by  H2SO4;  poorer  glass  by  boiling  HC1,  HNOs,  and 
aqua  regia.  (Berzelius.) 

Cone.  HNOs  does  not  act  on  flint  glass  at  145-150°. 
(Sorby,  C.  R.  50.  990.) 

Glass  of  ordinary  chemical  apparatus 
gives  up  traces  of  metals  to  HC1  and  HNO3+ 
Aq,  but  hard  Bohemian  glass  consisting  of 
75%  SiO2,  15%K2O,  10%  CaO,  resists  the 
action  of  warm  cone,  acids;  also  an  easily 
fusible  Na  K  glass  with  77  %  SiO2,  7.7% 
K2O,  5%  Na2O,  10.3%  CaO,  is  not  easily 
attacked.  (Stas.) 

KOH,  and  NaOH+Aq  dissolve  SiO2  from 
glass  the  more  easily  the  hotter  and  the  more 
cone,  the  solutions  are.  (Miiller.)  NH4OH, 
and  (NH4)2CO3+Aq  attack  many  kinds  of 
glass,  especially  flint  glass.  CaO2H2  attacks 
a;lass  appreciably  at  45°  and  lower;  still  more 
strongly  on  boiling.  (Lamy,  A.  ch.  (5)  14. 
155.) 

The  action  of  various  solvents  on  the  glass 
mentioned  on  page  359  in  Emmerling's  ex- 
periments is  as  follows: 

The  action  of  HCl+Aq  containing  0.2  to 
3%  HC1  is  practically  null,  but  is  increased 
either  by  dilution  or  concentration.  A  very 
small  quantity  (0.02%)  HC1  added  to  H2O 
almost  wholly  prevents  its  action  on  glass. 
With  HCl+Aq  (11%  HC1)  a  decrease  of  4.2 
mg.  was  noticed  in  the  first  hour,  and  only 
3-4  mg.  afterwards.  The  same  is  the  case  for 
3NO3+Aq  in  still  greater  degree,  0.008% 
HNO3  sufficing  to  nearly  counteract  the 
solvent  action  of  H20. 

H2SO4-f  Aq  has  about  double  the  solvent 
effect  possessed  by  H2O. 

Oxalic  and  acetic  acids  both  diminish  the 
solvent  action  of  H2O. 

The  addition  of  even  traces  (0.04%)   of 


362 


GLASS 


Na2CO3  increases  the  solvent  action,  and  this 
is  further  rapidly  increased  by  an  increase  in 
the  amount  of  Na2CO3.  Na2CO3+Aq  con- 
taining 1%  Na2CO3  dissolves  about  10  times 
as  much  as  pure  H2O,  i.  e.  about  35  mg.  per 
hour. 

The  above  is  also  the  case  with  KOH+Aq, 
but  in  even  greater  degree.  KOH+Aq  con- 
taining 0.025%  KOH  dissolved  three  times  as 
much  as  pure  H20. 

(NH4)2CO3+Aq  has  about  the  same  action 
as  H2O. 

With  NH4OH+Aq  (9%  NH3)  7  mg.  de- 
crease for  the  first  hour,  and  3  mg.  afterwards 
was  noticed.  The  concentration  of  the 
NH4OH+Aq  was  apparently  without  effect. 

The  addition  of  NH4C1  decreases  the  solv- 
ent action  of  H2O  proportionately  to  the 
amount  added,  but  with  new  flasks  large 
amounts  are  dissolved. 

With  NH4Cl+Aq  (7%NH4C1)  4.2  mg.  were 
dissolved  in  the  first  hour,  and  the  amount 
dissolved  gradually  decreased  to  null  after  24 
hours  on  account  of  the  liberation  of  HC1  by 
the  decomp.  of  NH4C1. 

NaCl,  KC1,  KNO3,  and  Na2SO4  show  a 
similar  behaviour  to  that  of  NH4C1. 

Na2HPO4+Aq  containing  0.4%  Na2HPO4 


has  six  times  the  solvent  action  of  pure  H20. 
but  the  action  is  not  increased  by  further 
concentration. 

In  general,  those  salts  the  acids  of  which 
form  insol.  Ca  salts,  as  Na2CO3,  Na2SO4, 
Na?HPO4,  (NH4)2C2O4,  increase  the  solvent 
action  of  H2O,  and  this  effect  is  greater  the 
more  concentrated  the  solution.  KC1, 
KN03,  NH4C1,  and  CaCl2  decrease  the  effect, 
and  the  stronger  the  solution  the  less  is  the 
action. 

All  Na  glass  with  approximately  the  above 
composition  has  the  same  power  of  resistance 
against  H2O;  Bohemian  K  glass  shows  a 
greater  resistance,  especially  against  acids. 
(Emmerling,  A.  160.  257.) 

Action  of  various  reagents  on  hard  Bohemian 
glass.  100  ccm.  substance  dissolved  mg. 
glass  in  6  days  at  100°. 

H2O  .  .  .10.0 
H2S+Aq  •''»  >  .  8.7 
Dil.  (NH4)2S+Aq.  .  52.5 
Cone.  (NH4)2S+Aq.  47.2 
Conc.NH4OH+Aq  .  42.5 
Dil.NH4OH+Aq.  .  7.7 
NH4SH+Aq.  .51.2 

(Cowper,  Chem.  Soc.  41.  254.) 


Action  of  various  solutions  on  glass  of  different  composition.    (The  figures  denote  decrease 
in  weight  in  mg.  of  a  100  ccm.  flask.) 


Time 

1 

2 

3 

4 

5 

6 

7 

8 

9 

10 

H20   . 
H2S04+Aq  (25%  H2S04)  . 
HCl+Aq  (12%  HC1) 
NH4OH+Aq  (10%  NH3)  . 
Na2HPO4+Aq  (12%  Na2HPO4) 
Na2CO8+Aq  (2%  Na2C03) 

5  hrs. 
3 
3 
3 
3 
3 

62 
'85 

283 

31 
43 

ie>6 

29 
35 
27 
62 
81 
130 

17 
8 
4 
11 
64 
124 

13 

7 
2 
8 
40 
50 

9 
6 
1 
•  7 
35 
45 

7 
5 
1 
7 
34 
42 

7 
5 
1 
6 
30 
42 

5 
5 
0 
5 
15 
26 

4 
3 
0 
5 
12 
25 

Composition  of  above  varieties  of  glass. 


i 

2 

3 

4 

5 

6 

7 

8 

9 

10 

Si02      .        . 
A1203    . 
CaO      . 
K2O      . 
Na2O    . 

76.22 
4^27 
19]  51 

74.09 
0.40 
5.85 
7.32 
12.34 

76.39 
0.50 
5.50 
4.94 
12.67 

68.56 
1.85 
7.60 
2.24 
19.75 

74.48 
0.50 
7.15 
6.64 
11.23 

74.69 
0.45 

7.85 
8.64 
8.37 

66.75 
1.31 
13.37 
05.50 
3.07 

74.12 
0.50 
8.55 
4.86 
11.97 

77.07 
0.30 
8.10 
3.75 
10.78 

74.40 
0.70 
8.85 
4.40 
11.65 

It  is  seen  that  glass  which  resists  the  attack 
of  H2O  also  resists  acids  and  alkalies,  and  that 
the  relative  resistance  of  all  varieties  to  any  of 
the  solutions  is  the  same.  Therefore  the 
action  of  H2O  may  be  accepted  as  a  criterion 
for  judging  of  the  resistance  of  a  glass  to  all 
solvents.  Glass  No.  10,  in  which  the  molecu- 
lar ratio  of  SiO2:CaO:K2O(Na2O)  is  8: 1:1.5,  is 
recommended  as  best  suited  for  chemical 
uses.  (Weber  and  Sauer,  B.  25.  70.) 

Mylius  and  Forster  (B.  25.  97)  recommend 
a  glass  in  which  the  molecular  ratio  of 
SiO2:  CaO:  K2O  (Na2O)  is  7.2:  1:  1.1  as  the 
best  suited  for  chemical  apparatus. 


In  an  exhaustive  research  on  the  action  of 
aqueous  solutions  on  glass,  which  cannot  be 
given  in  full  on  account  of  its  great  length, 
the  following  conclusions  are  reached: — 

1.  Solutions  of  caustic  alkalies  act  on  glass 
much  more  strongly  than  H2O,  dissolving  all 
the  constituents  ot  the  glass — that  is,  the  glass 
as  such.    Very  dilute  solutions  form  an  ex- 
ception. 

2.  Ot  the  caustic  alkalies,  NaOH+Aq  has 
the    strongest    action,    then    come    KOH, 
NH4OH,    and    BaO2H2+Aq    in    the    order 
named. 

3.  Increase  in  temperature  increases  the 


GLUCINUM  STANNIC  CHLORIDE 


363 


strength  of  the  attack  of  alkalies  very  con- 
siderably. 

4.  At  high   temperatures,    the   ease  with 
which   glass   is   attacked   increases   at   first 
rapidly  with  the  concentration  of  the  alkali, 
but  afterwards  more  slowly. 

5.  At  ordinary  temperatures  very  concen- 
trated alkali  solutions  have  less  action  on 
glass  than  dil.  solutions. 

6.  Solutions  of  pure  alkalies,  if  not  too 
cone.,  act  less  on  glass  than  when  contamin- 
ated with  small  amounts  of  SiO2. 

7.  Alkali     carbonates +Aq     attack     glass 
much  more  than  H2O,  even  when  they  are 
very  dilute.    The  action  corresponds  less  to 
that  of  the  caustic  alkalies  than  to  that  of 
other  salts.    With  equivalent  concentration, 
Na2CO3-f  Aq  has  a  stonger  action  than  K2CO3 
+Aq. 

8.  The  action  of  salt  solutions  on  glass  is  a 
compound  one,  depending  both  on  the  con- 
centration and  the  kind  of  salt  dissolved,  and 
is  made  up  of  the  action  of  the  H2O  and  the 
salt  in  solution. 

9.  Each  kind  of  attack  is  differently  in- 
fluenced by  the  composition  of  the  glass. 

10.  Solutions  of  those  salts,  the  acids  of 
which  form  insol.  Ca  salts,  have  a  stronger 
action  than  H2O,  and  the  action  increases 
with  the  concentration. 

11.  Solutions  of  those  salts,  the  acids  of 
which  form  sol.  Ca  salts,  have  less  action 
than  H20,  and  the  action  decreases  with  the 
concentration.    (Forster,  B.  25. 2494.) 

Data  on  this  subject  published  since  the 
first  edition  of  this  work  have  not  been  con- 
sidered. 

Glucinic  acid. 

Potassium  glucinate,  K2G1O2. 

Very  deliquescent.  Sol.  in  H2O  and  acids. 
(Kriiss  and  Moraht,  B.  23.  733.) 

Glucinum  (Beryllium),  Gl. 

Not  attacked  by  hot  or  cold  H2O.  Sol.  in 
cold  dil.  HNOs+Aq.  (Wohler,  Pogg.  13. 
577.) 

Sol.  only  in  boiling  cone.  HNO3+Aq. 
(Debray,  A.  ch.  (3)  44.  5.) 

Sol.  in  dil.  HCl+Aq.  dil.  and  cone.  H2S04+ 
Aq,  and  KOH+Aq,  but  insol.  in  NH4OH+ 
Aq.  (Wohler,  Debray.) 

Sol.  in  hot  HC1,  hot  cone.  HNO3,  and  hot 
cone.  H2SO4.  (Lebeau,  A.  ch.  1899,  (7), 
16.  474.) 

Glucinium  azoimide,  G1N3. 

Decomp.  by  hot  H2O.  (Curtius,  J.  pr. 
1898,  (2),  58.  292.) 

Glucinum  borocarbide,  3G12C,  B6C. 

Insol.  in  H2O.  Easily  sol.  in  mineral  acids 
especially  HN03.  (Lebeau,  A.  ch.  1899,  (7) 

16.481.) 


C4B6G16.    Stable  in  air. 
Easily  sol.  in  mineral  acids,  cone,  and  dil. 
(Lebeau,  C.  R.  1898,  126.  1349.) 


Glucinum  bromide,  GlBr2. 

Sol.  in  H2O  with  evolution  of  much  heat. 
(Wohler.) 

Sol.  in  abs.  alcohol.  (Lebeau,  A.  ch.  1899, 
(7)  16.  484.) 


Glucinum  carbide,  G12C. 

Decomp.  by  H2O.  Slowly  attacked  by 
cold  or  hot  cone.  HC1  and  HNO3.  Gradu- 
ally but  completely  sol.  in  dil.  acids.  (Le- 
beau, A.  ch.  1899,  (7),  16.  476.) 

G1C2.    Not  easily  decomp.  by  strong  acids. 

Easily  sol.  with  decomp.  in  dil  acids. 
(Lebeau,  C.  R.  1895,  121.  497.) 


Glucinum  chloride,  G1C12. 

Anhydrous.  Fumes  and  deliquesces  in  air. 
Sol.  in  H2O  with  hissing  and  evolution  of 
much  heat.  Easily  sol.  in  alcohol. 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 

Sol.  in  alcohol  and  ether.  SI.  sol.  in  C6H6, 
CHCls,  C14  and  CS2.  (Lebeau,  A.  ch.  1899, 
(7)  16.  493.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329.) 

+4H2O.    Very  hydroscopic. 

Easily  sol.  in  H2O  and  in  alcohol.  (Mie- 
leitner,  Z.  anorg.  1913,  80.  73.) 

Glucinum  chloride  ammonia,  G1C12,  4NHS. 
(Mieleitner,  Z.  anorg.  1913,  80.  73.) 

Glucinum  chloride  iodine  trichloride, 

2IC13,  G1C12+8H20. 

Hygroscopic.  (Weinland,  Z.  anorg.  1902, 
30.  140.) 

Glucinum  ferric  chloride,  G1C12,  FeCl3+H2O. 
Decomp.  by   H2O.     (Neumann,   A.   244. 
329.) 

Glucinum  mercuric  chloride,  G1C12,  3HgCl2  + 

6H2O. 
Sol.  in  H20.    (Atterberg,  B.  6.  1288.) 

Glucinum  thallic  chloride,  3G1C12,  2T1C13. 

Cryst.  from  HC1  solution.  (Neumann,  A. 
244.  348.) 

Glucinum  stannic  chloride. 
See  Chlorostannate,  glucinum. 


364 


GLUCINUM  FLUORIDE,  BASIC 


Glucinum  fluoride,  basic,  2G1O,  5G1F2. 

Solubility  of  freshly  pptd.  G1O2H2  in  NaOH  + 

Sol.  in  H2O.    (Lebeau,  A.  ch.  1899,  (7)  16. 

A  O  A     \ 

Aq  at  room  temperature. 

484.) 

millimols  Na  per  1. 

G.  G1O  dissolved  in  1  1. 

Glucinum  fluoride,  G1F2. 

649 

3.6 

Deliquescent.      Sol.    in    H2O.      Insol.    in 
anhydrous  HF.     Sol.  in  alcohol.     (Lebeau, 
C.  R.  1898,  126.  1421.) 

540 
540 

483 

ooo 

2.92 
2.53 
1.69 

1f\   A 

Sol.  in  H2O  in  all  proportions.    Somewhat 
sol.  in  abs.  alcohol.    Easily  sol.  in  90%  al- 

080 

388 

qon 

.64 
1.53 

1AJC 

cohol,  also  in  a  mixture  of  alcohol  and  ether. 

OoO 
qnrj 

.40 

1C)  A 

Insol.  in  anhydrous  HF.     (Lebeau,  A.  ch. 

oyu 

.  4*1 

1899,  (7)  16.  484.) 

In  the  first  two  cases  the  values  were  ob- 

Glucinum  potassium  fluoride,  G1F2,  KF. 

SI.  sol.  in  H2O.  (Awdejew.)  Much  more 
sol.  in  hot  than  cold  H2O.  (Berzelius.) 

G1F2,  2KF.  Sol.  in  about  50  pts.  H2O  at 
20°,  and  19  pts.  boiling  H2O.  (Marignac.) 


Glucinum  sodium  fluoride,  G1F2,  2NaF. 

Sol.  in  34  pts.  H2O  at  100°,  and  68  pts.  at 
18°.  (Marignac.) 

Glucinum  hydroxide,  G1O2H2. 

Easily  sol.  in  acids.     Sol.  in  H2SO3+Aq. 

Sol.  in  CO2+Aq;  100  com.  sat.  CO2+Aq 
dissolve  0.0185  g.  G1O.  (Sestini,  Gazz.  ch. 
it.  20.  313.) 

Also  sol.  in  KOH,  NaOH,  NH4OH,  or 
(NH4)2CO3+Aq,  especially  when  freshly  pre- 
cipitated; also  in  Na2CO3,  or  K2CO3+Aq. 
(Debray.) 

Insol.  hi  NH4OH+Aq  containing  NH4C1+ 
Aq. 

Very  si.  sol.  in  Li2CO3+Aq.    (Gmelin.) 

Sol.  in  H2SO4+Aq.    (Berthier.) 

Sol.  in  BaO2H2+Aa,  from  which  it  is  pptd. 
by  NH4  salts,  but  not  by  boiling.  Sol.  in 
boiling  NH4Cl+Aq  when  freshly  pptd. 

Sol.  in  NH4F+Aq.  (Helmholt,  Z.  anorg.  3. 
130.) 

Solubility  of  G1O2H2  in  NaOH+Aq. 


G.  Na  in  20  com. 


0.3358 

0.6717 
0.8725 
1.7346 


G.  Gl.  in  20  ccm. 


0.0358 

0.0882 
0.1175 
0.2847 


(Rubenbauer,  Z.  anorg.  1902,  30.  334.) 

When  glucinum  hydroxide  is  treated  with 
alkali,  more  dissolves  at  first  than  corresponds 
with  the  true  equilibrium  under  the  prevail- 
ing conditions,  for  such  solutions  spontane- 
ously deposit  more  or  less  glucinum  hydrox- 
ide according  to  the  concentration.  (Ruben- 
bauer.) 


tained  by  adding  to  GlCl2+Aq  at  0°,  ice  cold 
NH4OH  and  treating  the  ppt.  with  NaOH+ 
Aq.  In  the  remaining  cases  by  dissolving 
basic  G1CO3  in  HC1  and  pouring  into  NaOH  + 
Aq.  (Haber,  Z.  anorg.  1904,  38.  386.) 

Solubility  of  G1O2H2,  which  is  one  week  old' 
in  NaOH+Aq  at  t°. 


NaOH 


1-N 

2-N 


1-N 
2-N 


2-N 


20-23° 

20-23° 

20-23° 

50-53° 

50-53° 

50-53° 

100° 

100° 

100° 


G.  G1O  in  1  1. 


0.060 

0.170 
0.570 
0.080 
0.230 
0.900 
0.080 
0.290 
1.020 


(Haber.) 
Solubility  of  G1O2H2  in  NaOH+Aq  at  25C 


G.  mols. 


Na 


0.268 
0.318 
0.446 
0.526 
0.563 
0.801 
0.854 


Gl. 


0.0330 

0.0492 

0.0841 

0.089 

0.101 

0.143 

0.202 


(Wood,  Chem.  Soc.  1910,  97.  884.) 

Insol.  in  NH4OH+Aq  and  in  alkyl  amines. 
(Renz,  B.  1903,  36.  2753.) 

Sol.  in  GlSO4+Aq.  (Parsons,  J.  phys. 
Chem.  1907,  11.  658.) 

A  form  insol.  in  acids  and  alkalies  can  be 
obtained  by  sufficiently  long  heating  in  boil- 
ing H2O,  Na2CO3+Aq,  NH4OH+Aq,  or 
solutions  of  NaOH  or  KOH  so  dil.  that  the 
GIO2H2  is  either  insol.  or  very  si.  sol.  therein, 
(van  Oordt,  C.  C.  1906,  1.  108.) 

100  ccm.  of  glycerine+Aq  containing  about 
60%  by  vol.  of  glycerine  dissolve  0.1  g.  G1O. 
(Muller,  Z.  anorg.  1905,  43.  322.) 

Contains  VsHaO  (Schaffgotsch) ;  4/sH2O  (At- 
terberg). 


GLUCINUM  SELENIDE 


365 


Solubility  of  G1O2H2,  which  has  been  boiled  with  alkali,  in  various  solvents. 


Alkali  used 

Time 

Solvent 

Solubility 

10-N  NaOH 

NaOH 
NaOH 

23/Shrs. 

Long  time 
2hrs. 

0.106-X  XaOH 
0.39-X    XaOH 
0.97-X    XaOH 
2.0-X      XaOH 
2.0-X      XaOH 
10-X  K2CO2 
Dil.  HC1 
Hot  cone.  HC1 
Dil.  acetic  acid 

1  mol.  G1O2H2     331  mole  XaOH 
1  mol.  G1O2H2      183  mole  XaOH 
1  mol.  G1O2H2    91.8  mole  XaOH 
1  mol.  G1O2H2       49  mole  XaOH 
1  mol.  G1O2H2       49  mole  XaOH 
Insol. 
SI.  sol. 
Slowly  sol. 
Almost  insol. 

KOH 

TiU  flocculent 
ppt.  appeared 

1-X  KOH 

1-X  XaOH 
Warm  dil.  HC1 

Insol. 
it 

Sol. 

i^-N  Xa2C03 

f  Jf-X  Xa,CO,  for 
\  then  Vio-N  Na2CO3 
[     for 

3hrs. 
3  hrs.  and 
4hrs. 

1-X  XaOH 
Dil.  HC1 

1-X  XaOH 
Dil.  HC1 

Easily  sol. 

SI.  sol. 
Slowly  sol. 

i^-X  K2CO3 
10-X  K2CO3 

6  hrs. 
Short  time 

10-X  K,CO3 
1-X  XaOH 
Cold  10-X  K2CO3 

Insol. 
Easily  sol. 
Very  slowly  sol. 

XH4OH 

5  hrs. 

24-X  XaOH 

Very  si.  sol. 

(Haber.) 


Glucinum  iodide,  G1I2. 

Sol.  in  H20  with  evolution  of  much  heat. 
(Wohler.) 

Decomp.  in  moist  air  and  by  H2O. 

Sol.  in  abs.  alcohol.  Insol.  in  most  neutral 
organic  solvents,  as  benzene,  toluene,  etc. 
(Lebeau,  C.  R.  1898,  126.  1273.) 

Insol.  in  CeH6,  CvHs  and  oil  of  turpentine. 
Easily  sol.  in  CS2.  Sol.  in  anhydrous  alcohols 
without  evolution  of  heat.  (Lebeau,  A.  ch. 
1899,  (7)  16.  490.) 

Glucinum  iodide  ammonia,  2G1I2,  3XH3. 
Ppt.    (Lebeau,  A.  ch.  1899,  (7)  16.  492.) 

Glucinum  oxide,  G1O. 

Crystalline.  Insol.  in  acids  except  cone. 
H2SO4.  (Ebelmen,  C.  R.  32.  710.) 

Amorphous.  Absolutely  insol.  in  H2O. 
The  higher  the  temp,  to  which  the  substance 
has  been  heated  the  more  insol.  is  it  in  acids. 
Insol.  in  XH4OH+Aq  or  (XH4)2CO8+Aq. 
Insol.  in  cone.  XH4Cl+Aq,  or  KOH,  and 
XaOH+Aq.  (Rose.) 

When  obtained  by  ignition  of  G1SO4,  it  is 
very  slowly  but  completely  sol.  in  HC1,  and 
H2SO4+Aq.  (Rose.) 

Insol.  in  hydracids.  Sol.  in  cone.  H2S04. 
(Lebeau,  C.  R.  1896,  123.  819.) 

Insol.  in  liquid  XH3.  (Gore,  Am.  ch.  J. 
1898,  20.  828.) 


Glucinum  peroxide  basic,  2G1O2,  3G1O. 
+8KH2O.       (Komarovski,     Chem. 
1913,  104  (2)  707.) 


Soc. 


Glucinum  oxybromides. 

Sol.  in  H2O  if  three  or  less  equivalents  of 
base  are  present  to  one  of  acid;  insol.  if  more 
of  the  base  is  present.  (Ordway,  Am.  J.  Sci. 
(2)  26.  207.) 

Glucinum  oxychloride,  G12OC13  =  G1O,  GlClj. 
Insol.  in  H2O. 
3G1C12,   2G1O+2H2O   (?).     Sol.  in  H2O. 

GlCl2!r3G10+3H20  (?).  Sol.  in  H2O,.biit 
solution  soon  becomes  cloudy  and  deposits  a 
fine  ppt.  By  boiling  the  solution  it  is  decomp. 
into  above  salt,  and  G1C12,  12G1O2H2+ 
10H2O,  which  is  insol.  hi  H2O;  decomp.  into 
G1O2H2  by  washing.  Sol.  in  acids.  (Atter- 
berg.) 

Glucinum  oxyfluoride,  5G1F2,  2G1O. 

Readily  sol.  in  H2O.  (Lebeau,  C.  R.  1898,. 
126.  1419.) 

Glucinum  phosphide. 
Decomp.  by  H2O.    (Wohler.) 

Glucinum  selenide. 
SI.  sol.  in  H2O.    (Berzelius.) 


366 


GLUCINUM  SULPHIDE 


Glucinum  sulphide. 

Slowly  sol.  without  decomp.  in  H2O,  but 
easily  decomp.  by  acids.  (Wohler.) 

Gold,  Au. 

Gold  which  has  been  pptd.  from  AuCl3  + 
Aq  by  FeS04  is  si.  sol.  in  HC1.  (Awerkiew, 
Z.  anorg.  1909,  61.  10.) 

Not  attacked  by  H2O.  Insol.  in  HNO3  or 
HCl+Aq.  Easily  sol.  in  aqua  regia  or  any 
mixture  evolving  Cl  or  Br.  Sol.  in  selenic 
acid,  or  antimonic  acid+Aq;  less  easily  in 
arsenic  acid+Aq.  Sol.  in  mixtures  of  HC1 
and  nitrates,  or  HNO3  and  chlorides;  also  in 
(NaCl+KNO3+K2Al2(SO4)4)+Aq  (?).  Insol 
in  H2SO4,  except  in  presence  of  KMnO4, 
HNO3,  or  HIO3.  Sol.  in  a  solution  of  I  in 
ether  in  direct  sunlight. 

Sol.  in  solutions  of  ferric,  and  cupric  salts. 

Sol.  in  HCl+Aq  containing  H2CrO4, 
H2MnO4,  H2SeO4,  H3AsO4,  or  FeCl3.  (Wurtz). 

Attacked  by  fuming  HC1  (sp.  gr.  1.178)  at 
ord.  temp,  in  direct  light,  especially  in  the 
presence  of  a  trace  of  MnCl2,  but  not  attacked 
in  the  dark  even  in  the  presence  of  this  salt. 
(Berthelot,  C.  R.  1904,  138.  1298.) 

100  com.  hot  cone.  HC1  dissolve  0.008  g. 
yellow  Au  powder  in  4  hours.  (Hanriot  and 
Raoult,  C.  R.  1912,  166.  1086.) 

Upon  boiling  25  and  50  cc.  HCl+Aq  (sp. 
gr.  1.178),  dil.  to  125  cc.  with  250  mg.  sheet 
Au  x/s  in.  square,  0.009  in.  thick,  weighing 
250  mg.  for  several  hours,  there  was  no  loss 
of  weight  of  Au.  (McCaughey,  J.  Am.  Chem. 
Soc.  1909,  31.  1263.) 

From  5  g.  finely  divided  ordinary  yellow 
gold;  100  cc.  HNO3  of  22°  B.  dissolve  0.002  g. 

100  00.  HNO3  of  32°  B.  dissolve  0.0119  g. 
in  2  hrs. 

100  cc.  HNO8  of  36°  B.  dissolve  0.028  g. 
in  2  hrs. 

100  cc.  HNO3  monohydrate  dissolve  0.076 
g.  in  2  hrs.  (Hanriot  and  Raoult,  C.  R.  1912, 
166.  1085.) 

From  5  g.  brown  gold: 

100  ccm.  HNO8  of  22°  Baume  dissolve 
0.006  g.  in  2  hrs. 

100  ccm.  HNO3  of  32°  Baume  dissolve 
0.039  g.  in  2  hrs. 

100  ccm.  HNO3  of  36°  Baume  dissolve 
0.078  g.  in  2  hrs. 

100  ccm.  HNO3  monohydrate  dissolve  1.540 
g.  in  2  hrs.  (Hanriot  and  Raoult.) 

SI.  sol.  in  boiling  HNO3  (sp.  gr.  =  1.42). 
The  solution  deposits  Au  by  standing  several 
days.  (Dewey,  J.  Am.  Chem.  Soc.  1910,  32. 
320.) 

Best  composition  of  aqua  regia  for  dissolv- 
ing Au  is  200  cc.  HC1  (sp.  gr.  1.1946)  45  cc. 
HNO3  (sp.  gr.  1.4)  and  245  cc.  H20.  1  pt. 
Au  is  sol.  in  4.3  pts.  of  such  a  mixture. 
(Priwoznik,  C.  C.  1910,  II.  1743.) 

Sol.  in  1  pt.  HNO3+4  pts.  HC1  as  repre- 
senting the  most  economical  mixture.  (Pri- 
woznik, Chem.  Soc.  1911,  100.  (2),  484.) 


Easily  sol.  in  nitrosulphonic  acid  from  sul- 
phuric acid  manufacture,  when  mixed  with 
equal  parts  cone.  HCl+Aq.  (Borntrager, 
Rep.  anal.  Ch.  1887.  741.) 

Sol.  in  hot  cone.  H2SO4  in  the  presence  of 
MnO2,  Mn2O3,  Mn3O4,  PbO2,  Pb203,  Pb3O4, 
CrO3,  CrO4  and  Ni203.  Solution  also  takes 
place  slowly  in  the  cold.  Sol.  in  hot  H2SO4+ 
KMnO4.  Slowly  sol.  in  cold,  more  rapidly  in 
hot  H2SO4+HN03.  (Lenher,  J.  Am.  Chem. 
Soc.  1904,  26.  550.) 

Sol.  in  a  hot  solution  of  crystalline  telluric 
acid  in  H2SO4  or  H3PO4. 

Sol.  in  hot  H3PO4  in  the  presence  of  MnO2, 
Mn2O3,  Mn3O4,  the  higher  oxides  of  lead, 
CrO3,  chromium  tetroxide  and  nickelic 
oxide.  Solution  takes  place  more  slowly  in 
the  cold.  Sol.  in  hot  H3PO4  in  the  presence 
of  KMn04.  Slowly  sol.  in  a  cold,  more 
rapidly  sol.  in  a  hot  mixture  of  H3PO4  and 
HN03. 

Sol.  in  hot  arsenic  acid  in  the  presence  of 
MnO2,  Mn2O3  and  Mn3O4.  (Lenher,  J. 
Am.  Chem.  Soc.  1904,  26.  550.) 

Gold  leaf  is  not  attacked  by  cold  cone. 
H2SeO4,  when  completely  free  from  halogens, 
but  is  dissolved  by  cone.  H2SeO4  at  300°. 
(Lenher,  J.  Am.  Chem.  Soc.  1902,  24.  354.) 

Solubility  of  thin  sheet  Au  in  HC1  solution 
of  iron  alum. 


Mg.  Au  dissolved 

Time, 

hours 

lg.  Fe 

1  g.  Fe 

2g.  Fe 

2g.  Fe 

25  cc.  HC1 

50  cc.  HC1 

25  cc.  HC 

50  cc.  HC1 

Temp.  38-43°. 

16 

1.00 

1.30 

1.08 

1.47 

22 

1.12 

1.55 

1.20 

1.81 

40 

1.52 

2.15 

1.82 

2.75 

46 

1.71 

2.34 

2.02 

2.95 

64 

1.96 

3.10 

2.60 

3.79 

72 

2.  12 

3.30 

2.83 

4.05 

89 

2^32 

3.65 

3.22 

4.65 

100 

2.40 

3.76 

3.38 

4.81 

113 

2.45 

3.95 

3.51 

5.12 

124 

2.60 

4.09 

3.63 

5.39 

161 

2.78 

4.36 

3.95 

5.96 

185 

2.90 

4.49 

4.11 

6.22 

Temp.  98-100°. 

1 

1.13 

0.78 

1.15 

1.27 

2 

1.99 

1.74 

2.56 

2.86 

4 

3.46 

3.31 

4.55 

5.06 

16 

10.09 

11.37 

13.15 

15.56 

20 

12.20 

13.72 

15.59 

19.41 

24 

14.37 

16.49 

17.96 

23.29 

36 

17.38 

23.27 

22.07 

31.73 

42 

18.79 

26.30 

24.62 

35.29 

54 

20.94 

31.39 

29.49 

42.11 

59^ 

21.64 

33.12 

30.64 

44.43 

GOLD 


367 


The  solution  contained  the  given  amounts 
of  Fe  as  iron  alum,  the  sp.  gr.  of  the  HC1 
was  1.178,  and  the  solutions  diluted  to  125  cc. 
(McCaughey,  J.  Am.  Chem.  Soc.  1909,  31. 
1263.) 
The   solvent   action   of  ferric   salt   occurs 
even  in  presence  of  a  ferrous  salt,  but  de- 
creases   with    increase    of    concentration    of 
ferrous  salt.    (McCaughey.) 

Solubility  of  thin  sheet  Au  in  HC1  solution 
of  CuCl2. 

Solubility  of  Au  which  has  been  pptd.  from 
AuCl3-|-Aq  by  various  precipitants  in 
HCl+formaldehyde. 

HCHO 

(40%) 
ccm. 

HCl 

(1.19) 
ccm. 

Au  dis- 
solved 
g- 

Au  used  was 
pptd.  from 
AuCls+Aq.  by 

150 
100 
125 
100 
150 
250 
500 
100 
100 
100 
150 
250 
150 
100 
100 
100 

150 
100 
25 
200 
150 
250 
500 
500 
200 
200 
300 
125 
75 
200 
200 
100 

0.0007 
0.0006 
0.0008 
0.0009 
0.0003 
0.0002 
0.0008 
0 
0.0004 
0 
0.0006 
0.001 
0.0013 
0.0008 
0.0006 
0.0005 

FeS04 

a, 

(C 

sugar 

oxalic  acid 
n 

FeS04 
oxalic  acid 

a 

sugar 
ti 

FeS04 
it 

ECHO 

(( 

Time, 
hours 

Mg.  Au  dissolved 

1  g.  Cu 
25cc.HCl 

1  g.  Cu 
50  cc.  HC1 

2g.  Cu 
25  cc.  HC1 

2g.  Cu 

50  cc.  HC1 

Temp.  38-43°. 

19 
25 

43 

493^ 
66^ 
78 
91 
102 
139 
163 

0.03 

0.09 
0.10 
0.12 
0.11 
0.14 
0.14 
0.16 
0.18 
0.23 

0.26 
0.36 
0.54 
0.61 
0.76 
0.87 
0.92 
1.02 
1.34 
1.60 

0.05 
0.05 
0.14 
0.15 
0.17 
0.22 
0.24 
0.27 
0.32 
0.39 

0.39 
0.54 
0.94 
1.07 
1.40 
1.58 
1.75 
1.90 
2.45 
2.84 

180 
360 
360 
209 

540 
720 

720 
400 

0 
0.001 
0.0019 
0.0013 

FeS04 
sugar 
FeSO4 

In  the  last  four  cases  the  solubility  was 
determined  at  the  ordinary  temp.;  in  the 
first  sixteen  the  gold  was  boiled  with  the 
mixture  of  HCl  and  HCHO. 

(Awerkiew,  Z.  anorg.  1909,  61.  3.) 

Solubility  of  Au  in  boiling  HC1+ 
paraformaldehyde. 

Temp.  98-100°. 

1 
4 
16 
20 
26 
38 
43 
48 
60 

0.15 
0.55 
1.34 
1.63 
2.17 
3.13 
3.61 
4,07 
4.82 

0.34 
1.23 
5.00 
6.5? 
9.13 
13.98 
16.54 
19.26 
26.37 

0.17 
0.55 
2.12 

2.78 
3.59 
5.07 

5.77 
6.26 

7.47 

0.46 
1.35 
8.80 
11.86 
15.70 
23.14 
26.62 
30.80 
39.09 

(CH20)3 
g- 

HCl 

(1.19) 
g. 

Dissolved 
Au  g. 

Au  used  was 
pptd.  from 
AuCls+Aq.  by 

5 
5 
25 
20 
20 
20 
20 
20 
20 
40 
20 
20 
10 
10 
60 

25 
25 
125 
400 
400 
400 
400 
400 
400 
400 
300 
300 
200 
200 
120 

0.0005 
0.0004 
0.006 
0.0024 
0.0034 
0.003 
0.0065 
0.0044 
0.0005 
0.001 
0.0024 
0.003 
0.0008 
0.0006 
0.0015 

FeSO4 
oxalic'  acid 
sugar 
CHOH 

CH3OH 

u 

sugar 

formic  acid 
it 

CH3OH 
FeS04 

14 

CH8OH 
oxalic  acid 
FeS04 

Conditions  the  same  as  above  for  HC1+ 
iron  alum.    (McCaughey.) 

Finely  powdered  gold  is  sol.  in  cone  HC1 
in  the  presence  of  alcohol,  etc. 
0.0302  g.  Au.  is  sol.  in  100  cc.  HCl  +100  cc. 
CH3OH. 
0.0230  g.  Au.  is  sol.  in  100  cc.  HC1+100  cc. 
CHC13. 
0.0066  g.  Au.  is  sol.  in  100  cc.  HC1+100  cc. 
C2H5OH. 
0.0190  g.  Au.  is  sol.  in  100  cc.  HC1+100  cc. 
C5HnOH. 
0.0125  g.  Au.  is  sol.  in  100  cc.  HCl-f-50  cc. 
CC13CH(OH)2. 

(Awerkiew.) 

(Awerkiew,  C.  C.  1908,  II.  1566.) 


368 


GOLD 


Solubility  of  Au  in  boiling  HCl-f  methyl 
alcohol. 

Solubility  of  Au  in  boiling  HCl+phenol. 

CeHsOH 
g- 

HCl 

(1.19)  g. 

Dissolved 
Au  g. 

Au  used  was 
pptd.  from 
AuCb  +Aq.  by 

CHsOH 

(99%) 
ccm. 

HCl 

(1.19) 
ccm. 

Dissolved 
Au  g. 

Au  used  was 
pptd.  from 
AuCh+Aq.  by 

10+25 
10 
20 
25 
25 
50 
25 
25 

100 
40 
50 
100 
150 
200 
250 
250 

0.001 
0.0004 
0.0003 
0.0005 
0 
0.0005 
0.0005 
0.0012 

C6H6OH 

oxalic  acid 

u 

FeSO4 

HCOH 
u 

FeS04 

1C 

100 
150 
150 
25 
50 
50 
50 
50 
50 
100 
500 
1000 
50 
100 
100 
75 
90 
75 
80 
100 
100 
50 

100 
150 
150 
25 
50 
50 
50 
50 
50 
100 
500 
1000 
100 
200 
300 
25 
30 
25 
20 
50 
50 
200 

0.0302 
0.0043 
0.028 
0.001 
0.0002 
0.0005 
0.0002 
0.0015 
0.002 
0.0009 
0.0128 
0.0281 
0.0084 
0.0006 
0 
0.005 
0.005 
0.0014 
0.0005 
0.0018 
0.0008 
0.001 

FeSO4 
oxalic  acid 
sugar 
CH4OH 
oxalic  acid 
CH3OH 
oxalic  acid 

FeSO4 
u 

oxalic  acid 

FeS04 
it 

(i 
(i 
(i 

HCOH 

<( 

u 
tt 

FeSO4 
CH3OH 

it 

(Awerkiew.) 
Solubility  of  Au  in  boiling  HCl  +  chloroform. 

CHCh 

g. 

HCl 

(1.19) 
g. 

Dissolved 
Aug. 

Au  used  was 
pptd.  from 
AuCU+Aq.  by 

50 
100 
100 
150 
200 
250 
300 

100 
100 
100 
50 
400 
250 
300 

0.0009 
0.023 
0.0017 
.0.0012 
0.0024 
0.002 
0.0106 

FeS04 

a 

(i 
<i 

sugar 

u 

it 

(Awerkiew.) 

Solubility  of  Au  in  boiling  HCl  +  ethyl 
alcohol. 

(Awerkiew.) 

Colloidal  gold  is  sol.  in  dil.  alkalies.    (Paal, 
B.  1902,  35.  2236.) 
Rather  quickly  sol.   in   10-15%  solution 
I  in  KI+Aq. 
Very  slowly  sol.  in  5%  solution  of  I  in  KI  + 
Aq. 
Scarcely  sol.  in  more  dil.  solution  of  I  in 
KI+Aq. 
Easily  sol.  in  10%  NHJ+I.     Less  easily 
sol.  in  5%  NHJ+I.    (Boring,) 
Sol.  in  cold  Na2S+Aq  when  Na2S  is  present 
in  proportion  of  843  pts.  Na2S  to  1  pt.  Au. 
(Becker,  Sill,  Am.  J.  (3)  33.  199.) 
In  finely  divided  state  Au  is  sol.  in  boiling 
KCN+Aq.    Not  attacked  by  boiling  HgCl2 
+Aq.     (Vogel,  J.  pr.  20.  366.) 

Solubility  of  Au  (disks)  in  KCN+Aq  with 
(A)  oxygen  passed  through  solution,  and 
(B)  agitated  with  oxygen. 

C2H5OH 

(95%) 
ccm. 

HCl 
(1.19) 
ccm. 

Dissolved 
Au  g. 

Au  used  was 
pptd.  from 
AuCls+Aq.  by 

25 
100 
200 
150 
100 
100 
200 
250 
300 
1000 
150 

50 
200 
400 
50 
300 
100 
200 
250 
300 
1000 
150 

0.0006 
0.0111 
0.0017 
0.0003 
0.0004 
0.0015 
0.0055 
0.0021 
0.0197 
0.007 
0.008 

FeSO4 

« 

tt 

sugar 

(i 

C2H2OH 

sugar 
FeS04 

CH3OH 
tt 

(Awerkiew.) 

Solubility  of  Au  in  boiling  HCl+amyl 
alcohol. 

CsHuOH 

g- 

HCl 

(1.19) 
g. 

Dissolved 
Au  g. 

Au  used  was 
pptd.  from 
AuCls+Aq.  by 

-     %  KCN 

g.  Au  dissolved  in  24  hours 

A                                  B 

100 
100 
150 
100 
150 
300 
200 
500 

100 
200 
150 
100 
50 
100 
200 
500 

0.019 
0.0048 
0.0024 
0.0027 
0.0032 
0.0023 
0.0067 
0.028 

FeSO4 
tt 

sugar 
it 

FeS04 
CBHnOH 
FeS04 

1 
5 
20 
50 

0.00845                 0.0187 
0.01355                 0.0472 
0.0115                   0.0314 
0.00505                 0.108 

(Maclaurin,  Chem.  Soc.  1893,  63.  729.) 

The  solution  of  Au  in  KCN+Aq  is  es- 
sentially hastened  by  sunlight.      (Caldecott, 
Proc.  Chem.  Soc.  1904,  20.  199.) 

(Awerkiew.) 

GOLD  CHLORIDE 


369 


The  presence  of  oxygen  is  necessary  for 
the  solution  of  Au  in  KCN+Aq.  The  rate 
of  solution  of  Au  in  KCN+Aq  varies  with 
the  strength  of  the  solution,  being  small  for 
cone,  solutions,  increasing  .  as  the  solution 
becomes  more  dilute,  reaching  a  maximum  at 
0.25%  KCN,  and  then  again  diminishing. 
(Maclaurin,  Chem.  Soc.  1895,  67.  211.) 

Solubility  of  Au  (strips)  in  dil.  KCN+Aq. 


%KCN 

Mg.  Au  dissolved  in  24  hours 

0 

0.010 

0.0005 

0.043-0.07 

0.001 

0.10-0.23 

0.0016 

0.16 

0.002 

0.44 

0.00325 

1  77 

0.004 

4.29 

0.008 

48.43 

0.016 

74.96 

0.0325 

150.54 

0.065 

168.12 

(Christy,  Elektrochem.  Z.  1901,  7.  205.) 

Finely  divided  metallic  gold  is  completely 
sol.  at  the  ord.  temp,  in  solutions  of  potas- 
sium ferrocyanide.  Solution  takes  place 
very  slowly  even  when  the  potassium  ferro- 
cyanide solution  is  boiling.  (Beutel,  Z. 
anorg.  1912,  78.  158.) 

Sol.  in  RbCl4I+Aq.  (Erdmann,  Arch. 
Pharm.  1894,  232,  30.) 

Not  attacked  by  FeCI3+Aq  when  air  is 
excluded  but  very  energetically  attacked  in 
presence  of  HC1  and  oxygen.  (Mcllhiney, 
Am.  J.  Sci.,  1896,  (4),  2.  293.) 

Not  attacked  by  several  days  heating 
with  SOC12  at  150°.  At  200°  there  is  si. 
action  in  10  days.  (North,  J.  Am.  Chem. 
Soc.  1912,34.892.) 

SO2C12  in  excess  dissolves  pulverulent  Au 
by  several  hours  heating  at  160°.  (North, 
Bull.  Soc.  (4),  9.  647.) 

Sol.  in  PC13.  (Baudrimont,  A.  ch.  (4)  2. 
416.) 

Easily  sol.  in  acid  solutions  of  thiocar- 
bamide  especially  in  presence  of  suitable 
oxidizing  compounds.  (Moir,  Chem.  Soc 
1906,  89.  1345.) 

Gold  arsenide,  AuAs. 

H2O  or  alcohol  slowly  extracts  As;  HNO3+ 
Aq  converts  into  Au  and  HsAsO4.  Sol.  in 
aqua  regia.  Not  attacked  by  cold,  decomp. 
by  hot  cone.  H2SO4.  (Tivoli,  C.  C.  1887.  778; 
J.  B.  1887.  610.) 

Gold  bismuthide,  Au2Bi. 

Min.  Maldonite.    Sol.  in  aqua  regia. 

Aurous  bromide,  AuBr. 

Insol.  in  H2O.  (Thomsen,  C.  C.  1860. 
606.) 


Insol.  in  H20,  HNO3,  H2SO4. 

Sol.  in  NH4OH+Aq.  with  decomp. 

Decomp.  by  HBr  and  KBr+Aq.  Sol.  in 
KCN+Aq  without  decomp.  Slowly  decomp. 
by  alcohol,  ether,  acetone  and  moist  CHCI8. 
(Lengfeld,  Am.  Ch.  J.  1901,  26.  325.) 

Gold  (auroauric)  bromide,  Au2Br4. 
Not  deliquescent.    H2O  or  ether  dissolves 

out  AuBr3.    (Thomsen,  C.  C.  1860.  606.) 
Does  not  exist.    (Kriiss,  B.  20.  640.) 
Existence  is  maintained  by  Petersen.     (J. 

pr.  (2)  46.  334.) 

Auric  bromide,  AuBr3. 

Not  "deliquescent.  Slowly  sol.  in  H2O,  more 
readily  in  ether. 

Can  be  recryst.  from'AsBrs,  SbBr3,  TiBr2 
or  SnBr2.  (Lindet,  Bull.  Soc.  1886,  (2)  46. 
149.) 

Sol.  in  methyl  acetate.  (Naumann.  B. 
1909,  42.  3790.) 

Aurous  phosphorus  Zn'bromide,  AuBr,  PBr». 
Decomp.  by  H2O.    (Lindet,  J.  pr.  (2)  32. 

494.) 

Auric     phosphorus     pentabromide,     AuBr3, 

PBr5. 
Decomp.  by  H2O.    (Lindet.) 

Aurous     bromide     phosphorus     inchloride, 

AuBr,  PC13. 
Decomp.  by  H2O.    (Lindet.) 

Auric    praseodymium   bromide, 

PrBr3,  AuBr3+10H2O. 
Very  sol.  in  H2O;  sol.  in  cone  HBr.    (Von 
Schule,  Z.  anorg.  1898,  18.  355.) 

Aurous  bromide  ammonia, 
AuBr,  2NH3. 

Decomp.  by  H2O  and  dil.  HC1. 

Sol.  in  aqua  regia.  (Meyer,  C.  R.  1906, 
143.  281.) 

Gold  carbide,  Au2C2. 

Ppt.  Decomp.  by  boiling  H2O  without 
evolution  of  C2H2.  Decomp.  by  HC1  with 
evolution  of  C2H2.  (Mathews,  J.  Am.  Chem. 
Soc.  1900,  22.  110.) 

Aurous  chloride,  AuCl. 

Insol.  in  H2O,  but  gradually  decomp. 
thereby  into  Au  and  AuCl3.  (Thomsen,  J. 
pr.  (2)  13.  341.) 

Insol.  in  H2O  and  dil.  HNO3. 

Decomp.  by  cone.  HNO3  to  Au  and  AuCI3. 

Sol.  in  HC1,  HBr  and  in  sol.  of  alkali 
chloride  and  bromides,  with  decomp. 

Decomp.  by  alcohol,  ether  and  acetone. 
(Lengfeld,  Am.  Ch.  J.  1901,  26.  324.) 


370 


GOLD  CHLORIDE 


Gold  (auric)  chloride,  AuCl3. 

Deliquescent.  Very  sol.  in  H2O.  Sol.  in 
1.47  pts.  H2O.  (Abl.)  Sol.  in  cone.  HC1,  or 
HNOs+Aq  without  decomp. 

AsCl3  dissolves  about  22%  at  160°  and 
2.5%  at  15°.  Solubility  in  SbCl3  is  about  the 
same.  Much  less  sol.  in  SnCl4  or  TiCl4, 
SnCl4  dissolving  4%  at  160°  and  hardly  a 
trace  at  0°.  Very  si.  sol.  in  hot  or  cold  SiCl4. 
(Lindet,  Bull.  Soc.  (2)  46.  149.) 

SI.  sol.  in  liquid  NH3.  (Franklin  and  Kraus, 
Am.  Ch.  J.  1898,  20.  829.) 

Sol.  in  alcohol  with  gradual  decomp. 
(Gmelin.)  Sol.  in  ether  with  decomp.  in  light 
or  on  long  standing.  Ether  extracts  AuCl3 
from  AuCl3+Aq  (Proust).  Sol.  in  volatile 
oils  with  gradual  decomp. 

Sol.  in  ether.  (Mylius,  Z.  anorg.  1911,  70. 
207.) 

Very  sol.  in  ether.  (Willstatter,  B.  1903, 
36.  1830.) 

Completely  sol.  in  ether.  (Frank,  C.  C.. 
1913,  II.  541.) 

Insol.  in  or  decomp.  by  alcohol,  ether,  CS2, 
C6H6,  oil  of  turpentine,  pentane,  hexane, 
CHC13,  CC14,  ethyl  nitrate,  nitrobenzol, 
ethyl  acetate,  ethyl  propionate  and  pyri- 
dine.  (Lenher,  J.  Am.  Chem.  Soc.  1903,  26. 
1138.) 

.+2H2O.    (Thomsen.) 

Auroauric  chloride,  Au2Cl4. 

Decomp.  by  H2O  into  AuCl3  and  AuCl. 
(Thomsen,  J.  pr.  (2)  13.  357.) 

Does  not  exist.  (Kriiss  and  Schmidt,  J. 
pr.  (2)  38.  77.) 

Existence  is  maintained  by  Christensen. 
(J.  pr.  (2)  46.  328.) 

Auric  chloride  with  MCI. 
See  Chloraurate,  M. 

Auric  nitrosyl  chloride,  AuCl3,  NOC1. 

Sol.  in  H2O  with  decomp.  (Sudborough, 
Chem.  Soc.  59.  662.) 

Aurous  phosphorus  trichloride,  AuCl,  PC13. 
Decomp.  by  H2O.    Sol.  in  about  100  pts. 
PC13  at  15°,  and  about  8  pts.  at  120°.    Sol.  in 
AsCl3.    (Lindet,  C.  R.  101.  1492.) 

Auric  phosphorus  pentachloride,  AuCl3,  PC15. 
Decomp.  by  H2O.     Nearly  insol.  in  PC13. 
Sol.  in  AsCl3.    (Lindet.) 

Aurous  potassium  chloride,  AuCl,  KC1. 

Decomp.  by  H2O  or  HCl+Aq  into  KC1, 
KAuCl4,  and  Au.  (Berzelius.) 

Auric  potassium  chloride. 
See  Chloraurate,  potassium. 

Auric  selenium  chloride,  AuCl3,  SeCl4. 

Decomp.  by  H2O.  Sol.  in  AsCl3.  (Lindet, 
C.  R.  101.  1492.) 


Gold  (aurous)  sodium  chloride,  AuCl,  NaCl. 

Insol.  in  H2O.  Sol.  in  alcohol.  (Meillet, 
J.  Pharm.  3.  447.) 

Formula  is  4NaCl,  AuCl,  AuCl3.  (Jorgen- 
sen.) 

Auric  sodium  chloride. 
See  Chloraurate,  sodium. 

Auric  sulphur  chloride,  AuCl3,  SC14. 

Easily  decomp.  by  H2O.  (Lindet,  C.  R. 
101.  1492.) 

Aurous  chloride  ammonia,  AuCl,  NH3. 

Ppt.  Unstable.  (Diemer,  J.  Am.  Chem. 
Soc.  1913,  35.  554.) 

AuCl,  3NH3.  Decomp.  by  H2O  and  dil. 
acids. 

Sol.  in  aqua  regia.  Sol.  in  cone.  H2SO4 
with  decomp.  (Meyer,  C.  R.  1906,  143.  282.) 

AuCl,  12NH3.    (Meyer.) 

Auric  fluoride,  AuF3. 

Very  unstable. 

Is  incapable  of  existence  not  only  in  pres- 
ence of  H2O  but  under  the  ordinary  conditions 
met  with  in  the  laboratory .  and  in  nature. 
(Lenher,  J.  Am.  Chem.  Soc.  1903,  25.  1138.) 

Auric  hydroxide,  AuO3H3. 

Nearly  insol.  in  most  acids.  Easily  sol.  in 
very  cone.  HNO3+Aq  (Proust),  from  which 
all  AuO3H3  is  separated  by  dilution  (Fremy). 
Extremely  si.  sol.  in  fuming  HNO3.  Sol.  in 
dil.  HNO3+Aq  when  pure  (Kriiss,  A.  237. 
281).  Not  attacked  by  H3PO4.  Insol.  in  HF. 
Sol.  in  HC1,  or  HBr+Aq  (Fremy). 

Sol.  in  H2SeO4+Aq.    (Mitscherlich.) 

SI.  sol.  in  cone.  H2SO4;  somewhat  sol.  in 
HC2H2O3+Aq.  (Rose.) 

Nearly  insol.  in  cold  KOH+Aq,  but  dis- 
solved on  boiling.  Insol.  in  NH4OH+Aq  or 
alkali  carbonates  +  Aq  (Rose).  SI.  sol.  in 
boiling  CaCl2+Aq,  NaCl+Aq,  BaCl2+Aq 
(Pelletier).-  Sol.  in  NH4CN,  and  KCN+Aq 
(Himly). 

SI.  sol.  in  KC1,  or  NaCl+Aq.    (Pelletier.) 

Sol.  in  K4Fe(CN)6+Aq  at  ord.  temp, 
rapidly  on  boiling.  (Beutel,  Z.  anorg.  1912, 
78.  154.) 

AuO,  OH=Au2O3,  H2O.    (Kriiss.) 

Auroauric   hydroxide,   Au3O2(OH)2=3Au2O2 

+2H20. 

Insol.  in  boiling  cone.  KOH+Aq.  Decomp. 
by  cone.  HC1  or  HNO3+Aq  into  Au  and 
Au2O3,  which  dissolves.  (Schottlander,  A. 
217.  336.) 

Aurous  iodide,  Aul. 

Insol.  in  cold,  decomp.  by  hot  H2O,  H2SO4, 
HC1,  or  HNO3+Aq,  with  separation  of  Au. 
Decomp.  immediately  by  ether,  more  slowly 
by  alcohol. 


GOLD  POTASSIUM  SULPHIDE 


371 


Partially  sol.  in  KI,  FeI3,  or  HI+Aq 
(Pelletier).  SI.  attacked  by  NH4OH,  or 
NaCl+Aq  at  35°  (Fordos).  Instantly  de- 
comp.  by  KOH+Aq. 

Gold  (auric)  iodide,  AuI3. 

Insol.  in  H2O.  Sol.  in  alkali  iodides,  and 
HI+Aq.  Decomp.  on  air  or  by  alkalies. 
(Johnston,  Phil.  Mag.  J.  9.  266.) 

Aurous  iodide  ammonia,  Aul,  NH3. 

Decomp.  by  H2O  or  dil.  acids.  (Meyer, 
C.  R.  1906,  143.  281.) 

Sol.  in  aqua  regia. 

Aul,  6NH3.    (Meyer.) 

Aurous  oxide,  Au2O. 

Insol.  in  H2O  or  alcohol.  Decomp.  by  boil- 
ing with  HCl+Aq  into  Au  and  AuCl3. 
H2SO4,  HNO3,  or  HC2H3O2+Aq  do  not 
attack.  Sol.  in  cold  aqua  regia.  Sol.  in  HI 
+Aq.  Sol.  in  KOH,  or  NaOH+Aq  when 
freshly  precipitated.  (Berzelius.) 

According  to  Kriiss  (A.  237. 281)  all  hitherto 
prepared  Au2O  is  impure.  Pure  Au2O  is  sol. 
in  cold  H2O  when  freshly  precipitated,  from 
which  hydroxide  is  precipitated  by  boiling. 
Partly  sol.  in  HC1,  or  HBr+Aq.  Sol.  in 
KOH,  or  NaOH+Aq  when  freshly  precipi- 
tated. Not  affected  by  any  other  acid  or 
solvent.  (Kriiss.) 

The  so-called  solution"  of  Au2O  in  H2O  is 
in  reality  a  coloidal  suspension.  (Vanino,  B. 
1905,  38.  462.) 

Auric  oxide,  Au2O3. 
See  Auric  hydroxide. 

Auroauric  oxide,  Au2O2. 

Sol.  in  cold  HCl+Aq;  forms  insol.  comp. 
with  HF.  (Prat,  C.  R.  70.  842.) 

Obtained  pure  by  Kriiss  (A.  237.  296.) 

Gold  phosphide,  Au4P6. 

Not  attacked  by  HCl+Aq.  HNO3  forms 
H3PO4  and  leaves  undissolved  Au.  (Schrot- 
ter,  J.  B.  1849.  247.) 

AuP.  Decomp.  on  air  or  with  H2O.  (Ca- 
vazzi,  Gazz.  ch..  it.  15.  40.) 

Au3P4.  Readily  attacked  by  aqua  regia 
or  Cl2+Aq.  (Granger,  C.  R.  1897,  124.  498.) 

Gold  purple  (mixture  of  Au  and  SnO2). 

Insol.  in  H2O.    Easily  sol.  in  aqua  regia. 

HCl+Aq  dissolves  all  Sn  and  leaves  Au. 

Boiling  HNO?+Aq  dissolves  a  little  Sn. 

Insol.  in  boiling  KOH+Aq  (Berzelius). 
KOH+Aq  extracts  excess  of  SnO2,  and  the 
residue  becomes  sol.  in  H2O,  from  which  it  is 
pptd.  by  NH4Cl+Aq.  (Figuier,  A.  ch.  (3) 
11.  353.) 

Sol.,  when  still  moist,  in  NH4OH+Aq,  but 
insol.  if  it  has  been  dried. 

Obtained  in  colloidal  state  in  aqueous  solu- 
tion containing  0.58  g.  Au.  and  5.41  g.  SnO2 


in  a  litre.  This  solution  may  be  concentrated 
without  coagulation.  The  solution  is  coagul- 
ated by  dil.  HNO3,  or  HCl+Aq,  more  easily 
by  dil.  H2S04+Aq;  also  by  KC1,  HgCl2, 
FeSO4+Aq,  and  many  other  salts.  Not 
coagulated  by  alcohol,  but  easily  when  ether 
is  added  to  the  alcohol.  (Schneider,  Z.  anorg. 
5.  80.) 

Gold  (auric)  selenide,  Au2Se3. 

HNO3+Aq  dissolves  out  Se.  Sol.  in  aqua 
regia  or  alkali  sulphides  +  Aq.  (Uelsmann, 
J.  B.  1860.  90.) 

Aurous  sulphide,  Au2S. 

Easily  sol.  in  H2O  when  freshly  prepared, 
but  precipitated  from  aqueous  solution  by 
HC1,  KC1,  or  NaCl+Aq.  When  dried  is 
insol.  in  H2O. 

Insol.  in  boiling  dil.  or  cone.  HC1,  or  H2SO4 
+;Aq.  Easily  sol.  in  aqua  regia,  HCl+Aq 
with  KC1O3,  etc.  Slowly  sol.  in  alkali  mono- 
sulphides +Aq.  Easily  sol.  in  polysulphides 
+Aq. 

Insol.  in  KOH+Aq.  Sol.  in  KCN+Aq. 
(Kriiss,  B.  20.  2369.) 

Known  also  in  colloidal  state  in  aqueous 
solution  containing  1.74  g.  Au2S  per  1. 
(Schneider,  B.  24.  2241.) 

Auric  sulphide,  Au2S3. 

Insol.  in  H2O  and  acids  except  aqua  regia; 
sol.  in  alkali  sulphides,  or  KOH+Aq.  (Ber- 
zelius.) 

Does  not  exist  (Kruss,  B.  22.  2369),  but 
has  since  been  made  by  Antony  and  Luchesi 
(Gazz.  ch.  it.  20.  601).  Insol.  in  HC1,  or  dil. 
HNOs+Aq.  Decomp.  by  cone.  HNO3,  KOH. 
or  NaOH+Aq  with  separation  of  Au.  SI,, 
decomp.  by  NH4OH+Aq.  Easily  sol.  in 
KCN+Aq;  decomp.  by  (NH4)2S+Aq.  Sol. 
in  cold  Na2S  or  K2S+Aq;  decomp.  on  boil- 
ing. (Antony  and  Luchesi,  Gazz.  ch.  it.  21, 
2.  209.) 

Insol.  in  ether.  (Hofmann,  B.  1904,  37. 
246.) 

Auroauric  sulphide,  Au2S2. 

Insol.  in  H2O  or  acids  except  aqua  regia. 
SI.  sol.  in  cold  alkali  monosulphides  +  Aq, 
but  easily  sol.  on  warming.  Sol.  in  cold 
polysulphides  +  Aq,  but  less  in  ammonium 
polysulphide  than  the  other  alkali  poly- 
sulphides. 

Not  attacked  by  cold,  but  easily  sol.  in  hot 
KOH+Aq.  Sol.  in  KCN+Aq.  (Hoffmann 
and  Kriiss,  B.  20.  2704.) 

Obtained  also  in  colloidal  state  in  aqueous 
solution  containing  0.8  g.  per  1.  (Schneider.) 

Insol.  in  Na2S+Aq.  sat.  with  S.  (Ditte, 
A.  ch.  1907,  (8)  12.  273.) 

Aurous  potassium  sulphide,  Au2S,  3K2S. 

(Antony  and  Lucchesi,  Gazz.  ch.  it,  1896, 
26.  (2)  350.) 


372 


GOLD  SILVER  SULPHIDE 


Au2S,  4K2S-f-12H2O.  Very  sol.  in  H2O. 
(Ditte,  C.  R.  1895,  120.  322.) 

Gold  silver  sulphide,  Ag3AuS2. 

Ppt.  (Lucchesi,  Gazz.  ch.  it.  1896,  26. 
350-53.) 

Aurous  sodium  sulphide,  NaAuS+4H2O. 

Sol.  in  H2O  and  alcohol.  (Yorke,  Chem. 
Soc.  Q.  J.  1.  236.) 

+5H2O.  Sol.  in  H2O.  (Ditte,  C.  R.  1895,, 
120.  321.) 

Na3AuS2.  Sol.  in  H2O.  (Lucchesi,  Gazz. 
ch.  it.  1896,  26.  350-53.) 

Au2S,  2Na2S+20H2O.  Very  sol.  in  H2O. 
(Ditte,  C.  R.  1895, 120.  321.) 

Gold  telluride. 
Ppt.    (Berzelius,  Pogg.  8.  178.) 

Gold  silver  telluride,  Au2Te2,  Ag2Te. 

Min.  Sylvanite.  Sol.  in  HNO3+Aq  with 
separation  of  Au,  in  aqua  regia  with  separa- 
tion of  AgCl. 

3Ag2Te,  Au2Te.    Min.  Petzite. 

Hartshorn,  salts  of. 

See  Carbonate  carbamate,  'ammonium  hy- 
drogen. 

Helium,  He. 

Coefficient  of  absorption  for  H2O  at 
18.2°  =  0.0073.  (Ramsay,  Z.  phys.  Ch.  1906, 
55.  347.) 

Absorption  of  helium  by  H2O  at  t°  and  760 
mm.  pressure. 


t° 

Coefficient  of  absorption 

0 

0.01500 

0.5 

0.01487 

5 

0.01460 

10 

0.01442 

15 

0.01396 

20 

0.01386 

25 

0.01371 

30 

0.01382 

35 

0.01380 

40 

0.01387 

45 

0.01403 

50 

0.01404 

(Estreicher,  Z.  phys.  Ch.  1899,  31.  184.) 
Absorption  by  H2O  at  t°. 


't° 

Coefficient  of  absorption 

0 
10 
20 
30 
40 
50 

0.0134 
0.0100 
0.0138 
0.0161 
0.0191 
0.0226 

(Antropoff,  Roy.  Soc.  Proc.  1910,  83.  A  480.) 


Completely  insol.  in  benzene  and  in  alcohol' 
(Ramsay,  Chem.  Soc.  1895,  67.  684.) 

Hexamine  chromium  compounds. 
See  Luteochromium  compounds. 

Hexamine  cobaltic  compounds, 

Co2(NH3)6X6. 

See  Dichrocobaltic  compounds. 
Co(NH3)6X3. 
See  Luteocobaltic  compounds. 

Hexamine  indium  chloride,  Ir2(NH3)6Cl6. 
See  Irido/n'amine  chloride. 

Hexathionic  acid,  H2S6O6. 

Known  only  in  aqueous  solution,  which 
decomposes  rapidly,  even  in  presence  of  free 
sulphuric  acid.  (Debus,  A.  244.  76.) 

Potassium  hexathionate,  K2S6O4. 

Sol.  in  H2O,  with  rapid  decomp.  Not 
obtained  in  pure  state.  (Debus,  A.  244.  76.) 

Holmium,  Ho. 

Holmium  oxide,  Ho2O3. 

(Cleve,  C.  R.  89.  478;  91.  328.) 

Consists  of  at  least  two  elements.  (Lecoq 
de  Boisbaudran,  C.  R.  102.  1005.) 

Consists  of  seven  elements.  (Krtiss  and 
Nilson.). 

Ses?w?hydraurylamine,  (AuOH)3N,  NH3  = 

Au3N2+3H2O. 

Decomp.  by  boiling  with  H2O.  (Raschig, 
A.  235.  341.) 

Hydrazidophosphoric  acid. 

Barium  hydrazidophosphate, 

OP(N2H3)O2Ba. 
(Ephraim,  B.  1911,  44.  3420.) 

Lead  hydrazidophosphate,  OP(N2H3)O2Pb. 
Easily  sol.  in  HNO3.    (Ephraim.) 

Potassium  hydrazidophosphate, 

OP(N2H3)(OK)2.    (Ephraim.) 

Sodium  hydrazidophosphate, 

OP(N2H3)(ONa)2. 
Can  be  cryst.  from  dil.  alcohol.    (Ephraim.) 

Hydrazine,  N2H4=NH2— NH2. 

Very  sol.  in  H2O.     (Curtius,  B.  20.  1632.) 
Very  hydroscopic;  decomp.  by  H2O;  solv- 
ent   for    sulphur,    KC1,    KBr,    KNO3.     (de 
Bruyn,  R.  t.  c.  1894,  13.  433-40:  Chem.  Soc. 
1895,  68  (2)  347.) 

Mixes  in  all  proportions  with  alcohols; 
si.  sol.  in  organic  solvents.  (Lobry  de  Bruyn, 
Chem.  Soc.  1897,  72  (2)  22.) 


HYDRAZINE  HYDROIODIDE 


373 


Hydrazine  amidosulphonate, 

N2H4,  HSO3,  NH2. 

Very  sol.  in  H2O.  (Sabanejeff,  Z.  anorg. 
1899,  20.  22.) 

Hydrazine  azoimide,  N2H4,  HN3. 

Deliquescent.  Easily  sol.  in  H2O.  SI.  sol. 
in  alcohol,  and  can  be  crystallised  therefrom. 
(Curtius,  B.  24.  2344.) 

Hydrazine  borate,  (N2H4)2(B2O3)6. 

Sol.  in  H2O.  (Dschawachow,  C.  C.  1902, 
I.  1394.) 

(N2H4)2(H2B4O7)3.  Sol.  in  H2O.  (Dscha- 
wachow, C.  C.  1902,  I.  1394.) 

+5H2O.  Sol.  in  H2O.  (Dschawachow, 
C.  C.  1902.  1.  1394.) 

+  10H2O.  Ppt.  (Dschawachow,  C.  C, 
1902.  1.  1394.) 

Hydrazine  cuprous  bromide  chloride, 

N2H5C1,  N2H5  Br,  3CuBr. 
(Ranfaldi,  Real  Ac.  Line.  1906  (5)  16,  II, 

95.) 

Hydrazine  mercuric  bromide, 

HgBr2,  2  (N2H4,  HBr)+H2O. 
Very  sol.  in  H2O,  sol.  in  alcohol  and  acetone. 
SI.  sol.  in  acetic  ether. 

**  Insol.  in  ethyl  ether.     (Ferratini,   C.   A. 
1912.  1612.) 

Hydrazine  zinc  bromide,  2N2H4HBr,  ZnBr2 

+H20. 

Very  sol.  in  H2O;  sol.  in  alcohol  and  acetone. 
(Ferratini,  C.  A.  1912.  1612.) 

Hydrazine  carbonate. 

Very  deliquescent,  but  only  si.  sol.  in  H2O. 

SI.  sol.  in  alcohol.  (Curtius  and  Jay,  J. 
pr.  1889,  (2)  39.  41.) 

Hydrazine  zinc  carbonate  hydrazine, 

Zn(C02,  NH,  NH2)2,  2N2H4. 
Easily  sol.  in  H2O.    (Ebler  and  Schott,  J, 
pr.  1909,  (2)  79,  72.) 

Hydrazine  chlorate,  N2H4,  HC1O3. 

Very  sol.  in  H2O;  si.  sol.  in  alcohol.  Insol, 
in  ether,  CHC13  and  benzol.  (Salvadori, 
Gazz.  ch.  it.  1907,  37,  (2)  32.) 

Hydrazine  ^chlorate,  N2H4,  2HC1O3. 

Ppt.  Decomp.  in  aq.  solution.  (Turrentine, 
J.  Am.  Chem.  Soc.  1915,  37.  1123.) 

Hydrazine  cupric  chloride,  N2HSC1,  CuCl2-l- 


Decomp.  by  H20.     (Ranfaldi,  Real.  Ac. 
Line.  1906,  (5)  15,  II.  95.) 

+2H2O.     Decomp.  by  H2O.     (Ranfaldi.) 


Hydrazine^  mercuric  chloride,  N2H5C1,  HgCl2. 
(Hoffmann  and   Marburg,   A.    1899,  305. 

221.) 

Hydrazine  dithionate,  N2H4,  H2S2O6. 

Sol.  in  H2O;  decomp.  on  standing  in  aq. 
solution.  (Sabanejeff,  Z.  anorg.  1899,  20.  21.) 

2N2H4,  H2S206.    Sol.inH20.    (Sabanejeff.) 

Hydrazine  fluosilicate,  N2H4,  H2SiF6. 
Easily  sol.  in  H2O. 
Difficultly  sol.  in  ethyl  and  methyl  alcohol. 

(Ebler,  J.  pr.  1910,  (2)  81.  552.) 

• 

Hydrazine   fluotitanate,    (N2H4)2,   H2TiF6-b 

2H20. 

Ppt.  Sol.  in  H20.  (Ebler,  J.p  r.  1910,  (2) 
81.  555.) 

Hydrazine  monohydrobromide,  N2H4,  HBr. 

Very  easily  sol.  in  H2O  or  hot  alcohol. 
(Curtius  and  Schultz,  J.  pr.  (2)  42.  537.) 

Hydrazine  dihydrobromide,  N2H4,  2HBr. 

Easily  sol.  in  H2O.  SI.  sol.  in  alcohol. 
(Curtius  and  Schulz,  J.  pr.  (2)  42.  535.) 

Hydrazine  worcohydrochloride,  N2H4,   HC1. 
Extremely  sol.  in  H2O.    SI.  sol.  in  boiling 
absolute  alcohol.     (Curtius  and  Jay,  J.  pr. 
(2)  39.  38.) 

Hydrazine  (fthydrochloride,  N2H4,  2HC1. 

Easily  sol.  in  cold  H2O;  si.  sol.  in  hot 
alcohol.  (Curtius,  I.  c.) 

Sol.  in  2.67  pts.  H2O  at  23°.  Sp.  gr.  of  sat. 
solution  at  20° /4°  =  1.4226.  (Schiff,  Z.  phys. 
Ch.  1896,  21.  292.) 

Sp.  gr.  of  aqueous  solution  at  20°. 


%  salt 

Sp.  gr. 

25 
20 
15 
10 
5 

1.1183 
1.0923 
1.0675 
1.0436 
1.0203 

(Schiff,  Z.  phys.  Ch.  1896,  21.  292.) 

Nearly  insol.  in  hot  absolute  alcohol. 
(Curtius  and  Jay,  J.  pr.  (2)  39.  37.) 

Hydrazine  cfoTiydrofluoride,  N2H4,  2HF. 

Easily  sol.  in  H2O.  Nearly  insol.  in  alcohol. 
(Curtius  and  Schulz,  J.  pr.  (2)  42.  533.) 

Hydrazine  monohydroiodide,  N2H4,  HI. 
Easily  sol.  in  H2O.    (Curtius  and  Schulz.) 

Hydrazine  tfthydroiodide,  N2H4,  2HI. 

(Very  deliquescent.  Easily  sol.  in  H2O.  SI. 
sol.  in  alcohol.  (Curtius  and  Schulz,  J.  pr. 
(2)  42.  536.) 


374 


HYDRAZINE  HYDROIODIDE 


TnTiydrazine  cfthydroiodide,  3N2H4,  2HI. 

.    Easily  sol.  in  H2O  and  alcohol.     (Curtius 

and  Schulz,  J.  pr.  (2)  42.  540.) 

Hydrazine  hydroxide,  N2H4,  H2O. 

Miscible  with  H2O  or  alcohol,  but  not  with 
ether,  chloroform,  or  benzene.  (Curtius  and 
Schulz,  J.  pr.  (2)  42.  530.) 

Hydrazine  hypophosphate,  N2H4,  H4P2O6. 

SI.  sol.  in  H2O.  1.5  pts.  dissolve  in  100 
ptg.  H2O.  (Sabanejeff,  Z.  anorg.  1898,  17. 
490.) 

Hydrazine  hypophosphate  ammonia. 

N2H4,  H4P206,  NH3. 

Sol.  in  H2O.  (Sabanejeff,  Z.  anorg.  1899, 
20.  23.) 

Hydrazine  mercuric  iodide, 
2N2H6I,  HgI2+H2O. 

Very  sol.  in  H2O,  alcohol,  acetone,  acetic 
ether. 

Insol.  in  ether.  Excess  of  H2O  decomp. 
(Ferratini,  Gazz.  ch.  it.  1912,  42.  (1),  172.) 

Hydrazine  zinc  iodide, 

ZnI2,  2N2H4, 
Very  sol.  in  H2O;  sol.  in  alcohol  and  acetone. 
(Ferratini,  C.  A.  1912.  1612.) 

Hydrazine  nitrate,  N2H4,  HNO3. 

Very  sol.  in  H2O;  si.  sol.  in  abs.  alcohol. 
(Sabanejeff,  Z.  anorg.  1899,  20.  24.) 

Solubility  in  H2O  at  t°. 


t 

%  N2H4,  HClOi 

Sp.  gr. 

18 
35 

41.72 
66.9 

1.264 
1.391 

(Sommer,  Z.  anorg.  1914,  86.  85.) 

N2H4,  2HNO3.    Very  unstable. 

Sol.  in.H2O  but  solution  cannot  be  con- 
centrated beyond  30%  without  decomp. 

Decomp.  by  abs.  alcohol. 

Very  sol.  in  hydrazine  hydroxide +Aq. 
(Sabanejeff,  Z.  anorg.  1898,  20.  25.) 

Hydrazine  nitrite,  N2H4,  HN02. 

Very  sol.  in  H2O.  JPptd.  by  ether  from  solu- 
tion in  alcohol;  insol.  in  ether. 


Very  hydroscopic.    (Sommer,  Z.  anorg. 
1913,  83.  125.) 

Hydrazine  perchlorate,  N2H4,  HC104+2H2O. 
Sol.  in  1.48  pts.  H2O  at  30°  and  34  pts. 
alcohol;    crystallizes   from   boiling   absolute 
alcohol.    (Salvadori,  Ch.  Z.  31.  680.) 


+3H2O. 


Solubility  in  H2O  at  t°. 


(Carlson,  Dissert.  1910.) 

Hydrazine    efrperchlorate,   N2H4,   2HC1O4  + 
2H2O. 

Efflorescent. 
Deliquescent. 

102  pts.  salt  sol.  in  100  pts.  H2O  at  29°. 
2.8  pts.  salt  sol.  in  100  pts.  alcohol. 
l.Opt.      "      "  "  100    "     ether. 
(Turrentine,  J.  Am.  Chem.  Soc.   1915,  37. 
1123.) 

Hydrazine  phosphate,  N2H4,  H3PO4. 

Very  sol.  in  H2O.     (Sabanejeff,  Z.  anorg. 
1898,  17.  488.) 

N2H4, 2H3PO4.    Sol.inH2O.    (Sabanejeff.) 

Hydrazine  phosphite,  N2H4,  H3P03. 

Sol.  in  H2O.   (Sabanejeff,  Z.  anorg.  1898, 17. 
468.) 


t° 

g.  N2H4,  HNO3  per  100  g. 

Hydrazine  hydrogen  phosphite, 

Sat.  solution 

H20 

N2H4,2H3P03. 

T                            1          *            TT    S~\       A.1^                 j_T~                                     1               Ij. 

10 

63.63 

174.9 

ijess  soi.  in  ±i2u  tnan  tne  normal  salt. 
(Sabanejeff.) 

15 

68.47 

217.2 

20 

72.70 

266.3' 

Hydrazine  selenate,  N2H4,  H2SeO4. 

25 

30       . 
35 

76.61 
80.09 
83.06 

327.5 
402.2 
490.3 

Sol.  in  H2O  with  decomp.     (Rimini,  C.  C. 
1907,  I.  86.) 

40 
45 
50 
55 
60 

85.86 
88.06 
91.18 
93.58 
95.51 

607.2 
737.6 
1034. 
1458. 
2127. 

Hydrazine  zinc  selenate, 

(N2H6)2SeO4,  ZnSeO4. 
SI.  sol.  in  H20  but  more  sol.  than  Cu  salt. 
(Rimini  and  Malagnini,  Gazz.  ch.  it.  1907, 

37.  (1),  265.) 

Hydrazine  sulphocyanide,  N2H4,  HSCN. 

Very  deliquescent.  Sol.  in  H2O  and  alcohol. 
(Curtius  and  Herdenreich,  J.  pr.  1895,  [2]  52. 
488.) 

Hydrazine  sulphate,  N2H4,  H2SO4. 

Sol.  with  difficulty  in  cold,  easily  in  hot 
H2O.  Insol.  in  alcohol.  (Curtius,  I.  c.) 

100  pts.  H2O  dissolve  3.055  pts.  salt  at  22°. 
(Curtius  and  Jay,  J.  pr.  (2)  39.  39.) 

2N2H4,   H2SO4.     Very   deliquescent,    and 


HYDROGEN 


375 


sol.  in  H2O.    Insol.  in  alcohol.     (Curtius,  J 
pr.  (2)  44.  101.) 

Hydrazine  sulphite,  (N2H4)2H2S03. 
(Sabanejeff,  Z.  anorg.  1899,  20, 24.) 

Hydrazine  pyrosvlphite,  2N2H4,  H2S2O5. 

Sol.  in  H2O  with  decomp.;  insol.  in  alcohol 
(Sabanejeff,  Z.  anorg.  1899,  20.  23.) 

Hydrazine  thiosulphate,  (N2H4)2  H2S2O3. 

Ppt.  (Not  pure.)  (Ferratini,  Gazz.  ch 
it.  1912,  42.  (1)  138.) 

Hydrazine  lead  thiosulphate, 

PbS2O3,  2(N2H4)2H2S2O3+H2O. 

Insol.  in  H2O  and  alcohol. 

Sol.  in  HCl+Aq  and  in  HNO3+Aq, 
(Ferratini,  C.  A.  1912.  1612.) 

Hydrazine  silver  thiosulphate, 

Ag2S203,  (N2H4)2H2S203. 
Insol.  in  H2O;  sol.  in  NH4OH+Aq  and  in 
HNO3.    (Ferratini.) 

Hydrazine  sulphinic  acid. 

Barium  hydrazine  cfo'sulphinate, 

Ba2N2(SO2)2. 
Insol.  in  H2O;  sol.  in  acids.     (Ephraim, 
B.  1911,  44.  390.) 

Hydrazinesulphonic  acid,  N2H3SO2OH. 

Sol.  in  about  24  pts.  H2O  at  ord.  temp.  De- 
comp. by  mineral  acids;  nearly  insol.  in 
alcohol  and  other  organic  solvents.  (Traube, 
B.  1914,  47.  941.) 

Ammonium   hydrazinesulphonate, 

(N2H3S03)NH4. 

Deliquescent;  decomp.  by  acids.    (Traube.) 

Barium  hydrazinesulphonate, 

(N2H3S03)2Ba+2H2O. 
Sol.  in  H2O;  pptd.  by  alcohol;  decomp.  by 
acids.    (Traube.) 

Calcium  hydrazinesulphonate, 

(N2H3SO3)2Ca+H2O. 

Sol.  in  H2O.  Decomp.  by  acids.  Insol.  in 
alcohol.  (Traube.) 

Potassium  hydrazinesulphonate,  N2H3S03K. 
Decomp.  by  acids.    (Traube.) 

Silver  hydrazinesulphonate,  N2H3SO8Ag. 
(Traube.) 

Sodium  hydrazinesulphonate, 

N2H3SO3Na+H2O. 
Decomp.  by  acids.    (Traube.) 


Strontium  hydrazinesulphonate, 

(N2H3SO3)2Sr+2H2O. 
Sol.  in  H2O.    Decomp.  by  acids.    Insol.  in 
alcohol.    (Traube.) 

Hydriodic  acid,  HI. 
See  lodhydric  acid. 

Hydrobromic  acid,  HBr. 
See  Bromhydric  acid. 

Hydrochloric  acid,  HC1. 
See  Chlorhydric  acid. 

Hydrofluorboric  acid,  HBF4. 
See  Fluoborhydric  acid. 

Hydrofluoric  acid,  HF. 
See  Fluorhydric  acid. 

Hydrogen,  H2. 

SI.  absorbed  by  H2O. 

Sol.  in  150  pts.  H2O;  1  vol.  H2O  absorbs  0.016  vol.  H. 
Recently  boiled  H2O  absorbs  1.53%  H.  (Henry,  1803.) 

100  vols.  H2O  at  18°  absorb  4.6  vols.  H.  (de  Saussure, 
1814.) 

1  vol.  H2O  absorbs  0.0193  vol.  H  at  760  mm, 
and  all  temperatures  between  0°  and  23.6°. 
(Bunsen.) 

Later  work  does  not  confirm  the  above  state^- 
ment. 

Absorption  of  H  by  H2O  at  t  and  760  mm. 
0  =  coefficient  of  absorption;  0i  =  "solu- 
bility" (see  under  Oxygen). 


t° 

ft 

fr 

0 

0.02153 

0.02140 

1 

0.02134 

0.02120 

2 

0.02115 

0.02100 

3 

0.02097 

0.02081 

4 

0.02079 

0.02062 

5 

0.02061 

0.02043 

6 

0.02044 

0.02025 

7 

0.02027 

0.02207 

8 

0.02010 

0.01989 

9 

0.01994 

0.01971 

10 

0.01978 

0.01954 

11 

0.01962 

0.01937 

'  12 

0.01947 

0.01920 

13 

0.01932 

0.01904 

14 

0.01918 

0.01888 

15 

0.01903 

0.01872 

16 

0.01889 

0.01856 

17 

0.  -01876 

0.01840 

18 

0.01863 

0.01825 

19 

0.01850 

0.01810 

20 

0.01837 

0.01795 

21- 

0.01825 

0.01781 

22 

0.01813 

0.01767 

23 

0.01802 

0.01753 

24 

0.01791 

0.01739 

25 

0.01780 

0.01725 

26 

0.01770 

0.01712 

(Timofejeff,  Z.  phys.  Ch.  6.  147.) 

376 


HYDROGEN 


Absorption  of  H  by  H2O  at  t°  and  760  mm. 
0  =  coefficient  of  absorption. 

Absorption  of  hydrogen  by  H2O  at  t°  and  760 
mm.  pressure.  —  Continued. 

t° 

ft 

t° 

0            t° 

0 

t° 

0 

0i 

0 

0.0203 

16 

0.0182       32 

0.0161 

36 

0.01661 

0.01564 

1 

0.0202 

17 

0.0180       33 

0.0160 

37 

0.01657 

0.01554 

2 

0.0200 

18 

0.0179       34 

0.0159 

38 

0.01652 

0.01544 

3 

0.0199 

19 

0.0178       35 

0.0157 

39 

0.01648 

0.01535 

4 

0.0198 

20 

0.0177       36 

0.0156 

40 

0.01644 

0.01525 

5 

0.0196 

21 

0.0175       37 

0.0155 

41 

0.01640 

0.01515 

6 

0.0195 

22 

0.0174       38 

0.0154 

42 

0.01635 

0.01504 

7 

0.0194 

23 

0.0172       39 

0.0153 

43 

0.01631 

0.01493 

8 

0.0192 

24 

0.0171       40 

0.0152 

44 

0.01627 

0.01482 

9 

0.0191 

25 

0.0170       45 

0.0149 

45 

'0.01624 

0.01475 

10 

0.0190 

26 

0.0168       50 

0.0146 

46 

0.01620 

0.01460 

11 

0.0189 

27 

0.0167       60 

0.0144 

47 

0.01617 

0.01449 

12 

0.0187 

28 

0.0166       70 

0.0146 

48 

0.01614 

0.01437 

13 

0.0186 

29 

0.0164       80 

0.0149 

49 

0.01611 

0.01425 

14 

0.0184 

30 

0.0163       90 

0.0155 

50 

0.01608 

0.01413 

15 

0.0183 

31 

0.0162     100 

0.0166 

52 

0.01606 

0.01392 

KA 

o  01  fto^i 

001S6Q 

(Bohr  and  Bock,  W.  Ann.  44. 

318.) 

56 

0^01603 

.  V/AOUt7 

0.01343 

Absorption  of  hydrogen  by  H2O  at  t°  and  760 
mm.  pressure,     p  =  coefficient  of  absorp- 
tion.    0i  =  "  solubility"  (see  under  Oxy- 

58 
60 
62 
64 

0.01602 
0.01600 
0.01600 
0.01600 

0.01316 
0.01287 
0.01256 
0.01223 

gen). 

66 

0.01600 

0.01188 

t° 

0 

0i 

68 

0.01600 

0.01150 

70 

0  01600 

0.01109 

0 

0.02148 

0.02135 

72 

0.01600 

0.01065 

1 

0.02126 

0.02112 

74 

0.01660 

0.01017 

2 

0.02105 

0.02090 

76 

0.01600 

0.00966 

3 

0.02084 

0.02068 

78 

0.01600 

0.00912 

4 

0.02064 

0.02047 

80 

0.01600 

0.00853 

5 

0.02044 

0.02026 

82 

0.01600 

0.00790 

6 

0.02025 

0.02006 

84 

0.01600 

0.00723 

7 

0.02007 

0.01987 

86 

0.01600 

0.00652 

8 

0.01989 

0.01968 

88 

0.01600 

0.00575 

9 

0.01972 

0.01950 

90 

0.01600 

0.00494 

10 

0.01955 

0.01932 

92 

0.01600 

0.00407 

11 

0.01940      ' 

0.01915 

94 

0.01600 

0.00315 

12 

0.01925 

0.01899 

96 

0.01600 

0.00216 

13 

0.01911 

0.01883 

98 

0.01600 

0.00111 

14 

0.01897 

Of\"t  OOO 

0.01867 

Ortl  QP\1 

100 

0.01600 

0.0000 

15 
16 
17 

.  0188o 
0.01869 
0.01856 

.UloOl 

0.01836 
0.01821 

(Winkler,  B.  24.  99.) 

18 

0.01844 

0. 

01706 

19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 

0.01831 
0.01819 
0.01805 
0.01792 
0.01779 
0.01766 
0.01754 
0.01742 
0.01731 
0.01720 
0.01709 

ooooooooooo 

01792    . 
01777 
01761 
01746 
01730 
01715 
01700 
01685 
01670 
01656 
01642 

Critical   t,  —  232°.      (Natanson,    Z.    phys. 
Ch.  1895,  17.  43-48.) 
Coefficient  of  absorption  for  H2O=  0.01750 
at  25°;  0.01905  at  20°;  0.02059  at   15°; 
0.02213  at  10°;  0.02366  at  5°.     (Braun,  Z. 
phys.  Ch.  1900,  33.  734.) 
Solubility  in  H2O  at  25°  =  0.01926.     (Geff- 
cken,  Z.  phys.  Ch.  1904,  49.  267.) 
Coefficient  of  absorption  for  H2O  =0.01810 
at  20.11.°     (Hiifner,  Z.  phys.  Ch.  1907,  67. 

30 
31 
32 

0.01699 
0.01692 
0.01685 

0.01630 
0.01618 
0.01606 

Solubility    in    H2O     at    25°  =0.01962. 
(Drucker  and  Moles,  Z.  phys.  Ch.  1910,  75. 

A  1  *7  \ 

33 
34 
35 

0.01679 
0.01672 
0.01666 

p  p  p 

01596 
01585 
01574 

417.) 
Coefficient  of  absorption  for  H2O  at  15°  = 
0.01892;  at  20°=  0.01829.     (Muller,  Z.  phys. 
Ch.  1912,  81.  493.) 

HYDROGEN 


377 


Solubil 
S—  Solu 

ty  of  hydrogen  in  water  at  25°. 
bility  calculated  according  to  for- 
vhich  see  original  article, 
sure. 

Absorption  of  H2  by  HCl+Aq. 

mula,  for  T 

M 

S25° 

—  Pres 

0.426 
0.432 
1.063 
1.602 
1.802 
1.928. 
2.338 
2.438 
2.836 

0.01875 
0.01868 
0.01789 
0.01732 
0.01699 
0.01688 
0.01652 
0.01627 
0.01606 

p 

S 

P 

S 

756 
757 
850 

877 
986 
992 

0.0199 
0.0198 
0.0200 
0.0193 
0.0194 
0.0198 

1095 
1097 
1244 
1252 
1380 
1393 

0.0195 
0.0197 
0.0202 
0.0196 
0.0196 
0.0198 

(Findlay,  Chem.  Soc.  1912,  101.  1465.) 

Absorption  by  H2O  at  different  pressures. 
P  =  Hg-pressure  in  metres. 
X  =  coefficient  of  solubility. 
Table  I.  Volume  of  the  absorbing  liquid  = 
32.32  ccm.  T  =  19.5°. 

(Geffc 
Absorption  of  H2 

ken.) 
bYH2S°4l\q 

DJ       2 

M 

S25° 

0.527 
0.562 
0.985 
1.122 
1.866 
1.905 
2.605 
3.045 
3.174 
3.962 
3.989 

0.01869 
0.01838 
0.01780 
0.01768 
0.01642 
0.01632 
0.01575 
0.01496 
0.01456 
0.01422 
0.01402 

P 

X 

P 

X 

0.9010 
0.9967 
1.0809 
1.2133 
1.3711 
1.5448 
1.8002 
2.5208 
2.9971 

0.01798 
0.01796 
0.01799 
0.01800 
0.01794 
0.01791 
0.01793 
0.01793 
0.01795 

3.3926 
4.1405 
4.6629 
5.4705 
5.9580 
6.6507 
7.4548 
7.8783 
8.2439 

0.01789 
0.01776 
0.01761 
0.01748 
0.01725 
0.01706 
0.01674 
0.01652 
0.01632 

(Geffcken.) 
Solubility  of  H2  in  H2SO4+Aq  at  20°. 

Table  II.  Volume  of  the  absorbing  liquid  = 
32.007  ccm.    T  =  23°. 

%  HjSCh 

X20° 

p 

X 

P 

X 

0 
35.82 
61.62 
95.6 

0.0208 
0.00954 
0.00708 
0.01097 

1.1154 
1.3758 
1.7416 
2.1712 
2.8724 
3.4115 
4.0229 

0.01736 
0.01739 
0.01733 
0.01731 
0.01734 
0.01732 
0.01728 

4.6220 
5.1130 
5.9702 
7.1920 
7.4493 
7.8696 
8.1913 

0.01716 
0.01702 
0.01687 
0.01649 
0.01631 
0.01618 
0.01603 

(Christoff,  Z.  phys.  Ch.  1908,  65.  627.) 

Solubility  of  H2  in  colloidal  ferric  hydroxide 
solution  is  practically  the  same  as  its  solubility 
in  pure  H2O. 
Solubility  of  H2  in  a  solution  containing 
18.11  g.  Fe(OH)3  per  liter  at  25°  =  0.3085. 
Solubility  of  H2  in  a  solution  containing 
18.309  g.  Fe  (OH)3  per  liter  at  25°  =  0.3083. 
(Geffcken,  Z.  phys.  Ch.  1904,  49.  299.) 

Absorption  of  H2  by  bases  +Aq. 
M  =  content  in  gram-equivalents  per  liter. 
S  =  solubility.    (See  under  Oxygen.) 
Absorption  of  H2  by  KOH+Aq. 

(Cassuto,  Phys.  Zeit.  1904,  5.  235.) 

Absorption  of  H2  by  acids  +Aq. 
M  =  content  in  gram-equivalents  per  liter. 
S  =  solubility.    (See  under  Oxygen.) 
Absorption  of  H2  by  HNO3+Aq. 

M 

S 

25° 

0.741 
0.753 
1.22 
1.45 
2.09 
2.96 
3.18 
3.22 
4.13 
4.23 

0.01851 
0.01868 
0.01812 
0.01782 
0.01739 
0.01690 
0.01667 
0.01633 
0.01611 
0.01589 

M 

S25° 

0.536 
0.715 
1.059 
1.056 
1.480 

0.01658 
0.01539 
0.01378 
0.01389 
0.01195 

(Geffcken,  Z.  phys.  Ch.  1904, 

49.  267.) 

(Geffcken,  Z.  phys.  Ch.  1904,  49.  267.) 

378 


HYDROGEN 


Absorption  of  H2  by  NaOH+Aq. 

Absorption  by  salts  +Aq. 

M                                            S  25° 

Salt 

ti° 

Ik 

&^? 

d+^ 

02  . 

% 
salt 

t°2 

JjL 

a'S^ 

IF 

<5  ° 

Absorption- 
coefficient 
at  15° 
(Calculated). 

0.543                            0.01632 
0.571                            0.01608 
0.692                            0.01442 
0.974                            0.01409 
1.059                            0.01372 
1.137                            0.01348 
1.850                            0/01018 
3.400                            0.00648 
3.430                            0.00639 
4.687                           0.00483 

KC1 

15° 
15° 

1  .  1565 
1  .  1294 
1.0794 
1  .  0480 
1.0240 

22.92 
19.21 
12.13 
7.48 
3.83 

18.62 
18.82 
18.71 
19.00 
19.23 

0.00869 
0.00985 
0.01246 
0.01447 
0.01618 

0  .  00892 
0.01012 
0.01279 
0.01489 
0.01667 

KNOs 

1  .  1460 
1.1101 
1  .  0936 
1  .  0539 
1.0295 

21.46 
16.59 
14.26 
8.44 
4.73 

17.81 
17.27 
16.81 
17.58 
17.82 

0.01157 
0.01290 
0.01373 
0.01531 
0.01650 

0.01180 
0.01311 
0.01391 
0.01559 
0.01683 

(Geffcken.) 
Solubility  of  H2  in  salts  +Aq  at  15°. 

Salt 

%  Salt 

Coefficient  of 
absorption 

K2CO3 

15° 

1.4395 
1.3112 
1.2353 
1  .  1555 
1  .  0807 
1  .  0405 
1  .  0248 

41.81 
30.99 
24.13 
16.47 
8.83 
4.53 
2.82 

13.17 
12.77 
12  .  62 
12.51 
11.32 
12.29 
11.23 

0.00162 
0.00290 
0.00470 
0.00775 
0.01216 
0.01532 
0.01675 

0.00160 
0.00285 
0.00462 
0.00761 
0.01183 
0.01501 
0.01628 

H20 

0.00 

0.01883 

CaCl2 

3.47 
6.10 
11.33 
17.52 
26.34 

0.01619 
0.01450 
0.01138 
0.00839 
0.00519 

NaCl 

15° 

18° 

1.1817 
1  .  1088 
1.0807 
1.0315 

23.84 
14.78 
11.09 
4.47 

13.48 
13.17 
13.80 
13.56 

0.00602 
0.00938 
0.01140 
0.01565 

0.00595 
0.00925 
0..1130 
0.01548 

NaNOs 

1  .  2963 
1  .  2099 
1.1417 
1.0765 
1.0367 

37.43 
27.95 
19.77 
11.16 
5.57 

17.27 
17.36 
17.40 
17.65 
17.80 

0.00568 
0.00797 
0.01034 
0.01345 
0.01572 

0.00578 
0.00810 
0.01052 
0.01370 
0.01603 

MgS04 

4.94 
10.19 
23.76 

0.01501 
0.01159 
0.00499 

Na2CO3 

15° 

1.1213 
1.0835 
1  .  0457 
1.0217 

11.53 
8.02 
4.64 
2.15 

13.07 
12.08 
11.61 
11.94 

0.00851 
0.01106 
0.01420 
0.01677 

0.00839 
0.01082 
0.01385 
0.01639 

LiCl 

3.48 
7.34 
14.63 

0.01619 
0.01370 
0.0099 

Na2SO4 

18° 
15° 

1  .  1608 
1.0768 
1.0412 

16.69 
8.42 

4.58 

18.41 
18.57 
18.51 

0.00757 
0.01223 
0.01482 

0.00775 
0.01254 
0.01519 

K2CO3 

2.82 
8.83 
16.47 
24.13 
41.81 

0.01628 
0.01183 
0.00761 
0.00462 
0.00160 

LiCt 

15° 

1.0843 
1.0416 
1.0192 

14.63 
7.34 
3.48 

12.77 
12.40 
10.47 

0.01006 
0.01396 
0.01676 

0.00990 
0.01370 
0.01619 

MgS04 

15° 

1.2679 
1  .  1805 
1  .  1064 
1.0503 

23.76 
16.64 
10.19 
4.97 

18.26 
17.55 
17.30 
17.10 

0.00487 
0.00783 
0.01140 
0.01479 

0.00499 
0.00797 
0.01159 
0.01501 

KC1 

3.83 
7.48 
12.13 
19.21 
22.92 

0.01667 
0.01489 
0.01279 
0.01012 
0.00892 

ZnSO4 

18° 

1  .  3265 
1.1961 
1  .  1394 
1  .  0602 

26.51 
17.23 
12.73 
6.03 

18.56 
18.22 
17.95 

17.79 

0  .  00590 
0.00940 
0.01151 
0.01495 

0.00605 
0.00961 
0.01175 
0.01525 

KNO3 

4.73 
8.44 
16.59 
21.46 

0.01683 
0.01559 
0.01311 
0.01180 

CaClz 

15° 

1.2470 
1.2150 
1  .  1568 
1.0981 
1.0513 
1.0285 

26.34 
23.33 
17.52 
11.33 
6.10 
3.47 

17.68 
17.84 
18.09 
18.40 
18.04 
18.52 

0.00510 
0.00600 
0.00821 
0.01112 
0.01419 
0.01579 

0.00519 
0.00619 
0.00839 
0.01138 
0.01450 
0.01619 

NaNOs 

5.57 
11.16 
19.77 
37.43 

0.01603 
0.01370 
0.01052 
0.00578 

AlCls 

15° 

1.2647 
1  .  1589 
1.0914 
1  .  0488 

32.  30 
20.75 
12.46 

6.88 

17.14 
17.28 
17.30 
17.46 

0.00525 
0.00860 
0.01190 
0.01460 

0.00533 
0.00874 
0.01210 
0.01486 

Na2CO3 

2.15 
8.64 
11.53 

0.01639 
0.01385 
0.00839 

Ci2H22Oii 

17.5° 

1.2184 
1  .  1286 
1  .  0672 

47  .  65 
30.08 
16.67 

13.80 
14.19 
14.16 

0.00900 
0.01292 
0.01571 

0  .  00892 
0.01284 
0.01561 

(Steiner,  W.  Ann.  1894  (2),  62.  291.) 

Na2SO4 

4.58 
8.42 
16.69 

0.01519 
0.0154 
0.00775 

(Gordon,  Z.  phys.  Ch.  1895,  18.  14.) 

HYDROGEN 


379 


Solubility  in  salt  solutions. 
C  =  concentration  of  the  solution  in  terms 
of  normal. 

a  =  coefficient  of  absorption. 
Absorption  of  hydrogen  by  NH4NO3+Aq 
at  20°. 


p 

c 

a 

1.037 
2.167 
3.378 
4.823 
6.773 
11.550 

0.1308 
0.2765 
0.4363 
0.6333 
0.9069 
1.6308 

0.01872 
0.01845 
0.01823 
0.01773 
0.01744 
0.01647 

(Knopp,  Z.  phys.  Ch.  1904,  48.  103.) 
Absorption  of  hydrogen  by  KNO3+Aq  at  20° 


1.244 
2.094 
4.010 
5.925 

7.742 
13.510 


0.1245 
0.2114 
0.4127 
.0.6225 
0.8293 
1.5436 


0.01835 
0.01818 
0.01785 
0.01743 
0.01667 
0.01436 


(Knopp.) 

Absorption  of  hydrogen  by  NaNO3+Aq 
at  20°. 


Absorption  of  H  by  BaCl2  +Aq. 
at0  =  coefficient  of  absorption  at  tc 


Percent  of 

BaCh  in 

;he  solution 


7.002 
6.453 
3.600 
3.291 


a  25° 


0. 

0. 

0.01562 

0 


a20° 


a!5° 


014550.01591 
01474  0.01605 

0.017000.018390.01971 


017150.018330.01937 
01857  0.01957 
0.02089 
01570  0.01719  0.01847  0.01983  0.02110 


0 
0.01734 


a  10° 


(Braun.) 

1  vol.  alcohol  at  t°  and  760  mm.  absorbs  V 
vols.  H  gas  reduced  to  0°  and  760  mm. 


0.06925 
0.06910 
0.06896 
0.06881 
0.06867 
0.06853 
0.06839 
0.06826 
0.06813 


0.06799 
0.06787 
0.06774 
0.06761 
0.06749 
0.06737 
0.06725 
0.06713 
0.06701 


0.06690 
0.06679 
0.06668 
0.06657 
0.06646 
0.06636 
0.06621 


(Bunsen's  Gasometry,  p.  286.) 

One  vol.  alcohol  absorbs  0.06925 — 
0.000148t  +  O.OOOOOH2  vols.  H  at  t°. 
(Bunsen.) 

Solubility  in  alcohol +Aq  at  20°  and  760  mm. 


1.041 
2.192 
4.405 
6.702 
12.637 


0.1236 
0.2634 
0.5416 
0.8442 
1.7394 


0.01839 
0.01774 
0.01694 
0.01518 
0.01300 


wt.  % 

alcohol 


(Knopp.) 
Absorption  of  hydrogen  by  KCl+Aq  at  20°. 


0 

9.09 
16.67 
23.08 


Vol.  H2 
absorbed 


93 

.43 
29 
17 


wt.  % 

alcohol 


28.57 
33.33 
50 
66.67 


Vol.  H2 


1.04 
1.17 
2.02 
2.55 


(Lubarsch,  W.  Ann.  1889,  (2)  37.  525.) 
Absorption  of  hydrogen  by  alcohol. 


1.089 
2.123 
4.070 
6.375 
7.380 
13.612 


0.1475 
0.2907 
0.5687 
0.9127 
1.0682 
2.1222 


0.01823 
0.01757 
0.01661 
0.01531 
0.01472 
0.01255 


(Knopp.) 

Absorption  of  H2  by  NaCl+Aq. 
at0  =  coefficient  of  absorption  at  t°. 


Percent  of 
NaCl  in 
the  solution 

025° 

a20° 

al5° 

a!0° 

a5° 

5.999 
5.506 
4.496 
3.798 
1.523 
1.250 

0.01383 
0.01395 
0.01429 
0.01476 
0.01603 
0.01621 

0.01528 
0.01532 
0.01587 
0.01623 
0.01754 
0.01771 

0.01640 
0.01665 
0.01714 
0.01760 
0.01896 
0.01914 

0.01749 
0.01769 
0.01817 
0.01876 
0  .  02030 
0.2052 

0.01839 
0.01861 
0.01920 
0.01977 
0.02155 
0.02180 

(Braun,  Z.  phys.  Ch.  1900,  33.  735.) 


0 
6.2 


Coeff .  of 
absorption 


0.0676 
0.0693 


13.4 

18.8 


Coeff.  of 
absorption 


0.0705 
0.0740 


(Timofejeff.) 
Solubility  of  H2  in  ethyl  ether  at  t°. 


0 

5 

10 

15 


Solubility 


0.1115 
0.1150 
0.1195 
0.1257 


(Christoff,  Z.  phys.  Ch.  1912,  79.  459.) 

Coefficient  of  absorption  in  petroleum  = 
0.0582  at  20°,  and  0.0652  at  10°.  (Griewasz 
and  Walfisz,  Z.  phys.  Ch.  1.  70.) 


380 


HYDROGEN 


Absorption  of  hydrogen  by  chloralhydrate+ 
Aq  at  20°. 

Absorption  of  H2  by  glycerine  +Aq. 
t°  =  temp.  of  the  solution. 
P  =  %  glycerine  in  the  solution. 
/3t°  =  coefficient  of  absorption  at  t°. 
j815°  =  coefficient  of  absorption  at  15°. 

p 

C 

a 

4.911 
7.69 
14.56 
18.77 
29.50 
32.00 

0.310 
0.504 
1.030 
1.397 
2.530 
2.845 

0.01839 
0.01802 
0.01712 
0.01653 
0.01542 
0.01518 

t° 

P 

/St-     .    ' 

/315« 

14.5 
13.0 

13  8 

14.9 

22.8 
SR  n 

0.01654 
0.01532 
n  ni99fi 

0.01647 
0.01510 
n  0191fi 

(Knopp,  Z.  phys.  Ch.  1904,  48.  103.) 

Absorption  of  H2  by  chloralhydrate+Aq. 
t°=temp.  of  the  solution. 
P  =  %  chloralhydrate  in  the  solution. 
/3t°  =  coefficient  of  absorption  at  t°. 
/315°  =  coefficient  of  absorption  at  15°. 


t° 

p 

/3t° 

015° 

15.0 
16.4 
15.8 
15.0 
15.6 
16.2 
15.5 
15.0 

10.0 
16.1 
33.35 
39.4 
51.0 
60.8 
70.7 
79.0 

0.01740 
0.01719 
0.01475 
0.01470 
0.01300 
0.01281 
0.01282 
0.01320 

0.01740 
0.01737 
0.01484 
0.01470 
0.01306 
0.01230 
0.01287 
0.01320 

19.4 
17.4 
18.7 
16.5 
17.0 
17.2 
17.9 
18.3 

15.5 
28.3 
46.56 
52.0 
63.0 
66.0 
68.0 
78.4 

0.01732 
0.01569 
0.01388 
0.01314 
0.01270 
0.01285 
0.01286 
0.01398 

/320° 

0.01724 
0.01540 
0.01375 
0.01280 
0.01243 
0.01260 
0.01270 
0.01380 

(MOller,  Z.  phys.  Ch.  1912,  81.  499.) 
Solubility  of  H2  in  glycerol+Aq. 


t° 

%  glycerol 

Coefficient  of 
absorption 

14 

0 
2.29 
5.32 
8.57 
10.83 
15.31 

0.0193 
0.0189 
0.0186 
0.0182 
0.01815 
0.01765 

21 

0 
2.29 
5.68 
6.46 
10.40 
18.20 

0.0184 
0.0181 
0.0177 
0.0176 
0.0171 
0.0160 

(Henkel,  in  Landolt-Bdrnstein,  Tab.  4th  Ed. 
602.) 


(Muller,  Z.  phys.  Ch.  1912,  81.  496.) 


Solubility  of  H2  in  glycerine +Aq  at  25°. 
G  =  %  by  wt.  glycerine  in  the  solvent. 
S  =  Solubility  of  H2. 

P  =  corrected  pressure  at  end  of  experi- 
ment in  mm.  Hg  at  0°. 


p 

G 

s 

716.3 

4.0 

0.0186 

736.1 

10.5 

0.0178 

684.3 

22.0 

0.0154 

709.9 

49.8 

0.0099 

730.1 

50.5 

0.0097 

672.2 

52.6 

0.0090 

741.1 

67.0 

0.0067 

708.0 

80.0 

0.0051 

665.5 

82.0 

0.0051 

662.3 

88.0 

0.0044 

741.8 

95.0 

0.0034 

(Drucker  and  Moles,  Z.  phys.  1910,  75.  417.) 

Absorption  of  H2  by  glucose +Aq. 
t°  =  temp.  of  the  solution. 
P  =  %  glucose  in  the  solution. 
/3t°  =  coefficient  of  absorption  at  t°. 
^320°  =  coefficient  of  absorption  at  20°. 


t° 

p 

/St° 

/32(P 

20.5 
20.5 
21.1 
21.8 
21.2 

12.2 
20.7 
32.56 

45.8 
59.0 

0.01595 
0.01445 
0.01243 
0.01000 
0.00775 

0.01600 
0.01450 
0.01250 
0.01015 
0.00780 

(Miiller,  Z.  phys.  Ch.  1912,  81.  494.) 
Solubility  in  sugar+Aq  at  15°. 


%  Sugar 

Absorption  Coefficient 

16.67 
30.08 
47.65 

0.01561 
0.01284 
0.00392 

(Gordon,  Z.  phys.  Ch.  1895,  18.  14.) 


HYDROGEN  OXIDE 


381 


Absorption  of  H2  by  sucrose +Aq. 
t°=temp.  of  the  solution  in  the  absorption 


P  —  %  sucrose  in  the  solution. 

3t°  =  coefficient  of  absorption  at  t°. 


Absorption  of  H  by  organic  substances + 
Aq  at  t°. 

V  =  absorbed  volume  reduced  to  0°  and 
760  mm. 

a  =  coefficient  of  absorption. 


/318°  =  coefficient  of  absorption  at  15  . 

t° 

P                  £t° 

£15° 

12.7 
19.3 

0.01862 
0.01840 

0.01892 
/320°= 
0.01829 

15.2 
11.6 
12 
12.7 
11.8 
13.3 
12.6 

5.04         0.01723 
14.7           0.01547 
20.26         0.01500 
29.86         0.01290 
31.74         0.01220 
39.65         0.01047 
42.94         0.00956 

0.01726 
0.01510 
0.01462 
0.01257 
0.01185 
0.01033 
0.00939 

(Muller.) 

Absorption  of  H2  by  propionic  acid+Aq. 
at0  =  coefficient  of  absorption  at  t°. 

Percent  of 
propionic 
acid  in 
the  solutior 

a25°       a20° 
i 

a!5° 

alO3 

a5° 

9.910 
9.763 
6.500 
5.267 
3.373 
2.634 

0.016020.01782 
0.016380.01788 
0.016900.01829 
0.017050.01842 
0.017060.01866 
0.017220.01876 

0.  01908  ( 
0.  01929  ( 
0.  01925  ( 
0.  01983  ( 
0.  01987  ( 
0.2003    ( 

).  02029 
)  .  02042 
).  02093 
).  02117 
).  02120 
K02142 

0.02129 
0.02120 
0.02181 
0.02239 
0.02221 
0.02245 

(Braun,  Z.  phys.  Ch.  1900,  33.  735.) 

Absorption  of  H2  by  organic  acids  +Aq. 
M  =  content  in  gram-equivalents  per  liter. 
S  =  solubility. 
Absorption  of  H2  by  CH3COOH+Aq. 

M 

S25° 

0.517 
0.528 
1.160' 
1.20 
1.963 
1.980 
3.178 
3.220 
4.157 

0.01925 
0.01923 
0.01903 
0.01895 
0.01885 
0.01882 
0.01862 
0.01858 
0.01849 

(Geffcken,  Z.  phys.  Ch.  1904.  49.  267.) 
Absorption  of  H2  by  CH2ClCOOH+Aq. 

M 

S25° 

0.527 
0.990 
1.773 

0.01905 
0.01852 
0.01783 

(Geffcken.) 

Substance 


Glucose 

Glucose 

Glucose 

Urea 

Acetamide 

Alanine 

Glycocoll 


Grams 
in  1 
liter 


174 
80.8 
41.45 

60 

59 

89 

75  * 


Vol.  of 
solution 
used  in 


409.94 


20.28° 
20.16° 
20.00° 
20.17° 
20.11° 
20.08° 
20.16° 


V 

ccm. 


5.48 
6.12 
6.36 
6.26 
6.51 
5.57 
5.67 


0.01516 
0.01649 
0.01759 
0.01703 
0.01795 
0.01555 
0.01577 


(Hiifner,  Z.  phys.  Ch.  1907,  67.  623-4.) 
Solubility  in  organic  solvents. 


Solvent 

Solubility  at 
25°  C 

Solu- 
bility at 
20°  C 

ds 

dt 

Glycerine 

Not 

measurable 

Water 

0.01992 

0.02000 

—0.000016 

Aniline 

0.02849 

0.03033 

—0.000368 

Amyl  alcohol 

0.03708 

0.03533 

+0.00035 

Nitrobenzene 

0.03708 

0.03533 

+0.00035 

Carbon  bisulphide 

0.03753 

0.03358 

+0.00079 

Glacial  acetic 

0  .  06330 

0.06172 

+0.000316 

Benzene 

0.07560 

0.07071 

+0.000978 

Acetone 

0.07641 

0  .  07027 

+0.001228 

Amyl  acetate 

0.07738 

0.07432 

+0.00061 

Xylene 

0.08185 

0.07834 

+0.000702 

Ethyl  acetate 

0.08516 

0.07877 

+0.001278 

Toluene 

0.08742 

0  .  08384 

+0.000716 

Ethyl  alcohol 

0.08935 

0.08620 

+0.00063 

(99.8%) 

Methyl  alcohol 

0.09449 

0.09016 

+0.000866 

Isobutyl  acetate 

0.09758 

0.09287 

+0.000942 

Chloroform 
Carbon  tetra- 

Ino  constant 
value 

chloride 

(Just,  Z.  phys.  Ch.  1901,  37.  359.) 

Extended  investigations  have  been  made 
by  Findlay  and  Shen.  (Chem.  Soc.  1912, 
101.  1465)  on  the  effect  of  colloids  on  solu- 
bility of  H2  in  H2O.  See  original  article. 

Hydrogen  arsenide. 
See  Arsenic  hydride. 

Hydrogen  peroxide,  H2O2. 

Miscible  with  H2O.  Not  stable  in  cone, 
solution.  Aqueous  solution  gives  up  its  H2Oa 
to  ether.  Ethereal  solution  is  more  stable 
than  an  aqueous  solution  of  the  same  strength, 
and  may  be  distilled  without  decomp.  Mis- 
cible with  alcohol. 

Very  stable  in  aq.  solution  of  various 
cone,  if  perfectly  free  from  impurity  such  as 
compds.  of  heavy  metals,  etc.  (Woffenstein, 
B.  1894,  27.  3307.) 

Coefficient  of  distribution  between  ether 
and  H2O  determined  at  3°,  7°,  and  17.5° 
with  varying  quantities  (1.7 — 5%)  of  H2O2. 
(Osipoff,  C.  C.  1903,  II.  1265.) 

As  sol.  in  ether  as  in  H2O.  A  50%  solution 
in  H2O  still  contained  about  25%  H2O2  after 


382 


HYDROGEN  PHOSPHIDE, 


being  shaken  6  times  with  large  quantities  of 
fresh  ether. 

Insol.  in  petroleum  ether.  (Briihl,  B.  1895, 
28.  2855.) 

+H2O,  and  +2H2O.  Does  not  solidify  at 
-20°.  ( Wolff enstein,  B.  1894,  27.  3311). 

Hydrogen  phosphide,  gaseous  (Phosphine). 
PH3. 

Very  slightly  absorbed  by  H2O. 

Statements  as  to  solubility  in  H2O  vary 
considerably. 

(a)  Difficultly  inflammable  gas — 

1  vol.  H2O  absorbs  0.1122  vol.  PH3.  (Dyb- 
kowsky,  J.  B.  1866.  735.) 

1  vol.  H2O  absorbs  0.125  vol.  PH3.  (H. 
Davy.) 

(b)  Easily  inflammable  gas — 

1  vol.  H2O  absorbs  0.018  vol.  PH3.  (Gen- 
gembre,  Crell.  Ann.  1.  450.) 

1  vol.  H2O  absorbs  0.0214  vol.  PH3. 
(Henry.) 

1  vol.  H2O  absorbs  0.025  vol.  PH3.    (Davy.) 

1  vol.  H2O  absorbs  0.125  vol.  PH3.  (Dai- 
ton,  Ann.  Phil.  11.  7.) 

1  vol.  H2O  absorbs  0.255  vol.  PH3.  (Ray- 
mond, Scher.  J.  5.  389.) 

1  vol.  H2O  dissolves  0.26  vols.  PH3  at 
17°.  (Stock,  Bottger  and  Lenger,  B.  1909, 
42.  2855.) 

Sol.  in  cone.  H2SO4  without  immediate 
decomp.  (Buff,  Pogg.  16.  363.) 

1  vol.  50%  H2SO4  dissolves  0.05  vol.  PH3. 
(S.  B.  and  L.) 

Absorbed  by  CuSO4+Aq  and  by  Br. 
(Berthelot.) 

Absorbed  rapidly  by  Cu2Cl2+Aq  with 
formation  of  Cu2Cl2,  2PH3,  and  Cu2Cl2, 
4PH3.  (Riban,  C.  R.  88.  581.) 

1  vol.  alcohol  of  0.85  sp.  gr.  absorbs  0.5  vol.; 
1  vol.  ether  absorbs  2  vols.  (Graham.) 

Sol.  in  volatile  oils;  1  vol.  oil  of  turpentine 
absorbs  3.25  vols.  (Graham.) 

Several  varieties  of  blood  absorb  PH3. 

Hydrogen  phosphide,  liquid,  P2H4. 

Insol.  in  H2O.  Apparently  sol.  in  alcohol 
and  oil  of  turpentine,  but  solution  is  very 
quickly  decomp.  (Thenard,  A.  ch.  (3)  145.) 

Hydrogen  phosphide,  solid,  P4H2. 

Insol.  in  H2O  and  alcohol.  (Leverrier,  A. 
ch.  60.  174.) 

Insol.  in  all  liquids  except  liquid  PH2. 
(Thenard,  A.  ch.  (3)  14.  5.) 

Instantly  decomp.  by  HNO3,  or  H2SO4  + 
Aq.  Sol.  with  decomp.  in  alcoholic  solution  of 
KOH.  (Thenard.) 

Somewhat  sol.  in  liquid  phosphorus. 
(Buck,  Dissert.  1904.) 

P9H2.  Insol.  in  all  solvents.  (Stock, 
Bottger  and  Lenger,  B.  1909,  42.  2851.) 

Pi2H6.  Sol.  in  liquid  hydrogen  phosphide 
and  molten  P.  There  are  no  other  solvents 
which  appreciably  dissolve  it.  Insol.  in 
liquid  PH3.  (S.  B.  and  L.) 


t° 

Sol.  Coeff/ 

4 
9.65 
13.2 
22.5 

3  .  77  vols. 
3.43 
3.31 
2.70 

Hydrogen  selenide,  H2Se. 

More  sol.  in  H2O  than  hydrogen  sulphide. 
(Berzelius.) 

Solubility  coefficient  of  H2Se  at  t°. 


(Forcrand  and  Fonzes-Diacon,  C.  R.  1902, 
134.  171.) 

Sol.  in  cold  COC12.  (Besson,  C.  R.  1869, 
122.  140.) 

Hydrogen  silicide. 
See  Silicon  hydride. 

Hydrogen  sulphide,  H2S. 

(a)  Liquid.      Dissolves    S    on    warming, 
which  separates  on  cooling. 

(b)  Gas. 

1  vol.  H2O  absorbs  1.08  vols.  H2S  at  10°.  (Henry, 
1803.) 

1  vol.  H2O  absorbs  2.53  vols.  H2S  at  15°.  (de  Saus- 
sure,  Ann.  Phil.  6.  340.) 

1  vol.  H2O  absorbs  3  vols.  H2S  at  11°.  (Gay-Lussac 
and  Thenard.) 

1  vol.  H2O  absorbs  3.66  vols.  H2S  at  ord.  temp. 
(Thompson.) 

1  vol.  H*O  absorbs  2.5  vols.  H2S  at  ord.  temp. 
(Dalton.) 

1  vol.  H2O  absorbs  4.3706-0.083687t  + 
0.0005213t2  vols.  H2S  at  temperatures  be- 
tween 2  and  43.3°,  (Bunsen  and  Schonfeld, 
A.  93.  26.) 

At  0°  and  about  820  mm.  pressure,  1  ccm. 
H2O  absorbs  100  ccm.  H2S,  while  only  about 
4  ccm.  are  absorbed  at  ord.  pressure,  (de 
Forcrand  and  Villard,  C.  R.  106.  1402.) 

1  vol.  H2O  at  760  mm.  pressure  and  t°  absorbs 
V  vols.  H2S,  reduced  to  0°  and  760  mm. 


t° 

V 

t° 

V 

t° 

V 

0 

4.3706 

14 

3.3012 

28 

2.4357 

1 

4.2874 

15 

3.2326 

29 

2.3819 

2 

4.2053 

16 

3.1651 

30 

2.3290 

3 

4.1243 

17 

3.0986 

31 

2.2771 

4 

4.0442 

18 

3.0331 

32 

2.2262 

5 

3.9652 

19 

2.9687 

33 

2.1764 

6 

3.8872 

20 

2.9053 

34 

2.  1277 

7 

3.8103 

21 

2.8430 

35 

2.0799 

8 

3.7345 

22 

1.7817 

36 

2,0332 

9 

3.6596 

23 

2.7215 

37 

1.9876 

10 

3.5858 

24 

2.6623 

38 

1.9430 

11 

3.5132 

25 

2.6091 

39 

1.8994 

12 

3.4415 

26 

2.5470 

40 

1.8569 

13 

3.3708 

27 

2.4909 

(Schonfeld,  A.  93.  26.) 

HYDROGEN  SULPHIDE 


383 


Absorption  coefficient  of  H2S  in  H2O 
at  0°  =  4.6796.  (Prytz  and  Hoist,  W.  Ann. 
1895,  54,  137.) 

1  1.  H2O  dissolves  0.1004  mol.  H2S  at  25C 


Difficultly  sol.  in  cone.  H2SO4  with  decomp. 
Instantly  decomp.  by  fuming  HNOa. 
Solubility  of  H2S  in  HI+Aq  at  25°  and  760 


mm. 


64.  145.) 

HI  Mol.  per  1 

H2S  Mol.  per  1. 

Absorption  of  hydrogen  sulphide  by  H20  at  t°. 

0.00 
1.01 
1.51 
1.93 
2.65 
2.64 
3.42 
4.38 
5.005 
5.695 
6.935 
*(9.21 

0.1004 
0.111 
0.113 
0.125 
0.130 
0.138 
0.142 
0.163 
0.165 
0.181 
0.197 
0.267) 

t° 

Coefficient  of  absorption 

0° 
10° 
20° 

4.686 
3.520 
2.672 

[Gale.  fr.  data  of  Fauser.    (C.  C.  1889,  1. 
754.)] 
(Winkler,  Z.  phys.  Ch.  1906,  55.  350.) 

Absorption  of  hydrogen  sulphide  by  H2O  at  t°. 

*  Not  exact. 
(Pollitzer,  Z.  anorg.  1909,  64.  145.) 

Solubility  in  acids  +Aq. 
1  =  value  of  H2S  dissolved  .in  acid+Aq  as 
determined  by  titration. 
lo  =  value  of  H2S  dissolved  in  H2O  as  de- 
termined by  titration. 
t°=25°. 

t° 

Coefficient  of  absorption 

0 
10 
20 
30 
40 
50 
60 

4.621 
3.362 
2.  '554 
2.014 
1.642 
1.376 
1.176 

Acid 

l/lo 

(Winkler,  Z.  phys.  Ch.  1906,  55.  350.) 
Solubility  of  H2S  in  H2O. 

^-N.HCl 
H-N.H,SO4 

0.975 
0.905 

(McLauchlan, 

Less  sol.  in  IS 
H20. 
Sol.  in  CdCl2- 
Z.  anorg.  1894,  £ 

Solub 
1  —  value  of  E 

Z.  phys.  Ch.  1903,  44.  615.) 

'aCl,  or  CaCl2-f-Aq  than  in 

|-NH4OH+Aq.     (Crobaugh, 
.321. 

ility  in  salts  -fAq. 
2S  dissolved  in  salt+Aq  as 
tration. 
I2S  dissolved  in  H2O  as  de- 
ition. 

Layer  rich  in  H2S 

t° 

Mols.  H2S  per  100  mols.  H2O 

0 
6 
17 
26 
29.5 

0.4 
0.5 
0.8 
1.2 
1.6 

Layer  rich  in  H2O 

determined  by  t: 
lo  =  value  of  ] 
termined  by  titr 
t°  =  25°. 

t° 

Mols.  H2S  per  100  mols.  H2O 

29.4 
28.5 
26.9 
26.3 
23.8 
23.3 
22.9 
17.2 
13.7 
11.4 
5.3 

96.3 
96.9 
97.3 
97.5 
98.1 
98.1 
98.2 
98.8 
99.1 
99.25 
99.5 

Salt  +Aq. 

l/lo 

0.73 
0.78 
0.82 
0.847 
0.853 
0.960 
0.893 
0.913 
0.990 

Salt  +Aq. 

l/lo 

^-N.Na2SO4 
^-N.K2S04 
H-N.(NH4)«S04 
N.NaCl 
N.KC1 
.N.NH4C1 
N.NaNOa 
N.KNO3 
N.NH4NO8  . 

M-N.Na2SO4 
M-N.K2S04 
K-N.(NH4)2S04 
^-N.NaCl 
N.NaBr 
N.KBr 
N.NH4Br 
N.KI 

0.855 
0.890 
0.91 
0.930 
0.935 
0.945 
1.00 
0.98 

(Scheffer,  Proc.  K.  Ak.  Amsterdam,  1911,  14 
198.) 

(McLauchlan,  Z.  phys.  Ch.  1903,  44.  615.) 

384 


HYDROGEN  SULPHIDE 


Solubility  of  H2S  in  NaSH+Aq. 
(g.  mol.  H2S  dissolved  in  1 1.) 


t 

0.05  g.  mol. 
NaSH  per  1. 

0.1  g.  mol. 
NaSH  per  1. 

0.2  g.  mol. 
NaSH  per  1. 

15 
25 
35 
45 

0'.082 
0.064 

0.132 
0.104 
0.082 

0.129 
0.1035 

(Goldschmidt  and  Larsen,  Z.  phys.  Ch.  1910, 
71.  449.) 

At  18°  and  ord.  pressure,  100  vols.  alcohol  of  0.84 
sp.  gr.  absorb  606  mols.  H2S.  (de  Saussure,  1814.) 

1  vol.  alcohol  absorbs  17.89 l-0.65598t+ 
0.00661t2  vols.  H2S  between  0  and  22°. 
(Carius.) 

1  vol.  alcohol  at  t°  and  760  mm.  absorbs  V 
vols.  H2S  reduced  to  0°  and  760  mm. 


v 


17.891 
17.242 
16.606 
15.983 
15.373 
14.776 
14.193 
13.623 
13.066 


9 
10 
11 
12 
13 
14 
15 
16 
17 


12.523 

11.992 

11.475 

10.971 

10.480 

10.003 

9.539 

9.088 

8.650 


18 
19 
20 
21 
22 
23 
24 


8.225 
7.814 
7.415 
7.030 
6.659 
6.300 
5.955 


Solubility  in  organic  substances +Aq. 

1  =  value  of  H2S  dissolved  in  organic  sub- 
stance+Aq  as  determined  by  titration. 

lo=  value  of  H2S  dissolved  in  H2O  as  de- 
termined by  titration. 

t°=25°. 


Solution 


N-NH4C2H3O2 
N-C4H606 


N-(NH2)2CO 
pure  C8H6(OH)3 


l/lo 


1.09 

0.944 

0.858 

1.02 

0.863 


(McLauchlan,  Z.  phys.  Ch.  1903,  44.  615.) 
Solubility  in  acetic  acid+Aq  at  25°. 


Molecules  of 
CHaCOOH  in  100 

molecules 
CHsCOOH  +H2O 


0 

8.85 
16.7 
21.0 
35.5 
53.5 
55.7 
67.8 
81.0 
98.58 


Molecules  of  H2O 
in  100  molecules 
CHaCOOH  +H2O 


100 

91.15 

83.30 

79 

64.5 

40.5 

32^2 
19.0 
1.42 


l/lo 


1.00 
0.98 
0.955 


.00 

.035 

.21 

.29 

.40 

.83 


3.81 


(Carius,  A.  94.  140.) 
Solubility  in.alcohol+Aq  at  25°. 


Molecules  of 

C2H6OH  in  100 

molecules  C2H5OH 

+H20 


0.00 

1.60 

5.18 

9.25 

23.60 

47.75 

*(100 


Molecules  H2O  in 
100  molecules 
C2H5OH  +H2O 


100 

98  (?) 
94.82 
90.75 
76.40 
52.25 
0 


l/lo 


1.00 

0.96 

0.933 

0.91 

1.28 

1.95 

2.16) 


Carius. 


(McLauchlan.) 


Sol.  in  methyl  acetate  (Marchand),  ether 
(Higgins). 

Insol.  in  caoutchin. 

Sol.  in  glycerine  in  less  amount  than  in 
H2O.  If  a  certain  vol.  of  H2O  dissolves  100 
pts.  H2S,  the  same  vol.  of  glycerine  (1  pt. 
glycerine  +lpt.  H2O)  dissolves  only  60  pts. 
H2S,  but  the  solution  is  very  stable.  After 
standing  a  year  there  is  no  appreciable 
decomp.  (Lapage,  J.  Pharm.  (4)  5.  256.) 

According  to  Lindo  (C.  N.  57.  173),  the 
solution  in  glycerine  is  no  more  stable  than 
that  in  H2O. 

Sol.  in  CS2. 


(McLauchlan.) 
Hydrogen  persulphide,  H2S2  or  H2S5. 

Decomp.  by  contact  with  H2O,  in  which  it 
is  apparently  insol.  Sol.in  ether  with  subse- 
quent decomp.  Sol.  in  CS2.  (Thenard,  A. 
ch.  48.  79.) 

H2S2.  Quickly  decomp.  by  ether,  acetic 
ether,  ethyl,  or  amyl  alcohol.  H2S  has  no 
action. 

Cone.  HC1,  or  HC2H3O2+Aq  have  no  ac- 
tion. Sol.  in  a  solution  of  S  in  CS2,  and  in 
liquid  hydrocarbons. 

Chloroform  dissolves  without  decomp. 
(Sabatier,  C.  R.  100.  1346,  1585.) 

Alkalies,  and  K2S+Aq  decomp.  instantly. 

Decomp.  by  H2O,  dil.  and  cone.  HC1,  cone. 
H2SO4,  alkali  and  alcohol.  Sol.  in  alcohol 
containing  HC1  but  soon  decomp.  in  this 
solution.  Miscible  in  all  proportions  and 
without  decomp.  with  benzene,  ether  and  CS2. 
(Bloch,  B.  1908,  41.  1977.) 

Formula  is  H2S5.     (Rebs,   A.  246.  356.) 

+7H2O.  Easily  decomp.  by  heat,  (de 
Forcrand  and  Villard,  C.  R.  106.  1402.) 

Hydrogen  Zn'sulphide,  H2S3. 

Decomp.  by  H2O,  dil.  and  cone.  HC1,  cone. 
H2SO4,  alkali  and  alcohol.  Somewhat  sol.  in 
alcohol  containing  HC1,  but  slowly  decomp. 
in  this  solution.  Miscible  with  ether,  ben- 
zene and  ,CS2  and  these  solutions  are  relatively 
stable.  (Bloch,  B.  1908,  41.  1974.) 


HYDROXYLAMINE  COLUMBATE 


385 


Hydrogen  telluride,  H2Te. 

SI.  sol.  in  H2O.  Decomp.  in  the  air. 
(Ernyei,  Z.  anorg.  1900,  25.  313.) 

Hydrosulphuric  acid,  H2S. 
See  Hydrogen  sulphide. 

Hydrosulphurous  acid,  H2S02. 
,   See  Hyposulphurous  acid. 

Hydroxylamic  acid. 

Calcium  hydroxylamate,  Ca(ONH2)2. 

Very  explosive;  decomp.  by  H2O.  (Ebler 
and  Schott,  J.  pr.  1908,  (2)  78.  323.) 

Zinc  hydroxylamate  Zn(ONH2)2. 

Decomp.  by  H2O.    (Ebler  and  Schott.) 

Zinc  hydroxylamate,  hydroxylamine, 

Zn(H2NO)2,  3NH3O. 
Very  unstable. 
Insol.  in  abs.  alcohol.    (Ebler  and  Schott.) 

Hydroxylamine,  NH3O  =  NH2(OH). 

Known  only  in  solution. 

Sol.  in  alcohol.    (Lossen,  J.  pr.  96.  462.) 

Prepared  in  free 'state  by  de  Bruyn. 

Very  deliquescent,  and  sol.  in  H2O  and 
alcohol.  SI.  sol.  or  insol.  in  CHC13,  C6H6, 
ether,  or  ethyl  acetate. 

Methyl  alcohol  at  5°  dissolves  35%;  ethyl 
alcohol  at  15°,  15%;  boiling  dry  ether,  1.2%; 
boiline-  ethyl  acetate,  1.6%.  (de  Bruyn,  R. 
t.  c.  11.  18.) 

Hydroxylamine  arsenate,  As04H3(NH30)8. 

SI.  sol.  in  cold  H2O;  sol.  in  hot  H2O  from 
which  it  can  be  cryst.  (Hofmann,  A.  1899, 
307.  331.) 

Hydroxylamine  azoimide. 
See  Azcimide,  hydroxylamine. 

Hydroxylamine  bromide,  NH2OH,  HBr. 

Very  sol.  in  H2O;  insol.  in  ether  by  which 
it  is  pptd.  from  solution  in  alcohol.  (Adams, 
Am.  Ch.  J.  1902,  28.  205.) 

2NH2OH,  HBr.  Easily  sol.  in  H2O;  insol. 
in  ether  and  ligroin.  SI.  sol.  in  alcohol. 
(Adams.) 

Hydroxylamine  mercuric  bromide  hydroxyla- 
mine, 2NH2OH,  2HBr,  HgBr2, 2NH2OH. 
Decomp.  by  H2O  and  methyl  alcohol. 
Readily  decomp.  by  alkalies.    (Adams.) 

Hydroxylamine  calcium,  HO.Ca.ONH2. 

Partially  decomp.  by  H2O  at  ordinary 
temp.  (Hofmann,  Z.  anorg.  1898, 16.  464.) 


Hydroxylamine  chloride,  basic,  NH3(OH)C1, 
NH2OH. 

Sol.  in  H2O.  Alcohol  precipitates  from 
aqueous  solution.  Insol.  in  ether.  (Lossen.) 

2NH3(OH)C1,  NH2OH.  Deliquescent; 
very  sol.  in  H2O,  less  in  alcohol,  and  insol.  in 
ether.  (Lossen.) 

Hydroxylamine  chloride,  NH3(OH)C1. 

Not  deliquescent.  Very  sol.  in  H2O  and 
hot  ordinary  alcohol.  SI.  sol.  in  absolute  al- 
cohol. Insol.  in  ether.  (Lossen.) 

Sol.  in  1.2  pts.  H2O  at  17°.  (Schiff,  Z.  phys. 
Ch.  1896,  21.  290.) 

Sp.  gr.  of  aqueous  solution  at  17°. 


%  salt 

sp.  gr. 

40 

1.1852 

28 

1.1260 

20 

1.0888 

14 

1.0616 

10 

1.0437 

7 

1.0303 

5 

1.0214 

3.5 

1.0147 

(Schiff,  Z.  phys.  Ch.  1896,  21.  290.) 

100  pts.  absolute  methyl  alcohol  dissolve 
16.4  pts.  at  19.75°;  100  pts.  absolute  ethyl 
alcohol  dissolve  4.43  pts.  at  19.75°.  (de 
Bruyn,  Z.  phys.  Ch.  10.  783.) 

Somewhat  sol.  in  alcohol.  (Adams,  Am. 
Ch.  J.  1902,  28.  204.) 

Hydroxylamine  mercuric  chloride,  NH2OH, 
HC1,  HgCl2. 

Very  sol.  in  H2O  and  alcohol.  Less  sol.  in 
ether.  (Adams,  Am.  Ch.  J.  1902,  28.  213.) 

5(NH2OH)2,  HC1,  2HgCl2.  Sol.  in  cold' 
H2O,  alcohol  and  ether.  More  easily  sol.  in 
methyl  alcohol.  Sol.  in  HC1.  The  slightest 
trace  of  alkali  causes  decomp.  (Adams.) 

#ermhydroxylamine  cobaltic  bromide, 

[Co(NH2OH)6]Br3. 
(Werner,  B.  1905,  38.  897.) 

Zferahydroxylamine  cobaltic  chloride, 

[Co(NH2OH)6]Cl3. 

Very  stable  toward  HC1.  (Werner,  B. 
1905,  38.  895.) 

Hexahydroxylsanme  cobaltic  nitrate. 

[Co(NH2OH)6](N08)a. 
(Werner.) 

Zferahydroxylamine  cobaltic  sulphate, 

[Co(NH2OH)6]2(S04)3+2H20. 
Easily  sol.  in  H2O.    (Werner.) 


Hydroxylamine  columbate, 

Explosive.    SI.  sol.  in  H2O.    (Hofmann,  Z. 
anorg.  1898,  16.  473.) 


386 


HYDROXYLAMINE  DITHIONATE 


Hydroxylamine  dithionate,  (NH2OH)2, 

F2S206. 

Sol.  in  H2O;  decomp.  on  heating  the  aq. 
solution.  (Sabanejeff,  Z.  anorg.  1898, 17. 485.) 

Hydroxylamine  fluosilicate,  (NH3O)2,  H2SiF6 

+2H20. 

Easily  sol.  in  H2O.  Nearly  insol.  in  methyl 
and  abs.  ethyl  alcohol.  (Ebler,  J.  pr.  1908, 
(2),  78.  338.) 

Hydroxylamine  fluotitanate,  (NH3O)3,  H2TiF6 
Sol.  in  H2O.     SI.  sol.  in  methyl  alcohol. 
(Ebler,  J.  pr.  1908,  (2)  78.  340.) 

Hydroxylamine  hypophosphite, 

(NH8OH)H2P02. 

Very  sol.  in  H2O.  (Sabanejeff,  Z.  anorg. 
1898,  17.  483.) 

Sol.  in  H2O  and  absolute  alcohol.  Insol. 
in  ether.  (Hofmann  and  Kohlschiitter,  Z. 
anorg.  1898,  16.  469.) 

Hydroxylamine     potassium     hypophosphite, 

(H2P02)2(NH30)8K2. 

Easily  sol.  in  H2O,  decomp.  on  heating; 
sol.  in  hot  abs.  alcohol.  (Hofmann  and  Kohl- 
schiitter, Z.  anorg.  1898,  16.  468.) 

Hydroxylamine  hypophosphate, 

(NH3OH)2H2P2O6. 

Easily  sol.  in  H2O.  (Sabanejeff,  Z.  anorg. 
1898,  17.  489.) 

Hydroxylamine  iodide,  NH2OH,  HI. 

Hydroscopic;  sol.  in  methyl  alcohol.  Very 
explosive.  (Wolffenstein  and  Groll,  B.  1901, 
34.  2419.) 

ZHTiydroxylamine  iodide,  (NH2OH)2,  HI. 

Deliquescent.  More  sol.  in  H20,  methyl 
and  ethyl  alcohol  than  the  tri  compound.  Is 
decomp.  when  recryst.  from  these  solvents. 
Insol.  in  ether.  (Dunstan,  Chem.  Soc.  1896, 
69.  841.) 

Trihydroxylamine  iodide,  (NH2OH)3,  HI. 

Deliquescent  in  moist  air.  Sol.  in  H20, 
methyl  and  ethyl  alcohol.  Insol.  in  ether. 
(Dunstan.) 

Hydroxylamine  nitrate,  NH3(OH)NO3. 

Very  sol.  in  H2O  and  absolute  alcohol. 
(Lessen.) 

Hydroxylamine  or^Aophosphate, 

(NH3OH)3PO4. 
SI.  sol.  in  cold  H2O.    (Lessen.) 

Only  si.  sol.  in  H2O.  (Hofmann,  A.  1899, 
307.  330.) 

Moderately  sol.  in  H2O.  (Ross,  Chem.  Soc. 
1906,  90,  (2)  19.) 


Solubility  in  H2O. 

1  g.  of  aqueous  solution  contains  at: 
0°  10° 

0 . 012        0 . 015  g.  hydroxylamine  phosphate, 

20°  30° 

0 . 019        0 . 027  g.  hydroxylamine  phosphate, 

40°  50° 

0 . 040        0 . 055  g.  hydroxylamine  phosphate, 

60°  70° 

0.077        0. 102  g.  hydroxylamine  phosphate, 

80°  90° 

0. 133        0. 168  g.  hydroxylamine  phosphate. 
(Adams,  Am.  Ch.  J.  1902,  28.  204.) 

(NH3OH)H2PO4.  Hygroscopic.  Aq.  solu- 
tion is  decomp.  on  heating.  (Sabanejeff,  B. 
1897,  30.  287.) 

Hydroxylamine  phosphite,  (NH3OH)2HPO3. 

Sol.  in  H2O  and  absolute  alcohol.  (Hof- 
mann and  Kohlschiitter,  Z.  anorg.  1898,  16. 
467.) 

(NH3OH)H2PO3.  Sol.  in  H2O.  Insol.  in 
alcohol.  (Sabanejeff,  Chem.  Soc.  1900,  78, 
(2),  14.) 

Hydroxylamine  phosphite  ammonia, 

(NH3OH)H2PO3,  NH3. 
Sol.  in  H2O.    (Sabanejeff,  Chem.  Soc.  1900, 
78,  (2)  14.) 

Hydroxylamine  sodium,  NaONH2. 

Very  hygroscopic,  (de  Bruyn,  R.  t.  c. 
1892,  11.  18.) 

Hydroxylamine  sulphate,  (NH3OH)2SO4. 

Easily  sol.  in  H2O.  Precipitated  from  con- 
centrated aqueous  solution  by  alcohol.  (Los- 
sen.) 

Sol.  in  cone.  NH4OH+Aq.  Insol.  in  al- 
cohol and  ether.  (Preibisch,  J.  pr.  1873,  (2) 
7.  480.) 

Not  deliquescent.  Sol.  in  %  of  its  wt.  of 
H2O  at  20°.  (Divers  and  Haga,  Chem.  Soc. 
1896,  69.  1665.) 

1  g.  of  aqueous  solution  contains  at: 
—8°     0°     +10° 

0.307  0.329  0.366  g.  hydroxylamine  sulphate, 
20°      30°     40° 
0.413  0.441  0.482  g.  hydroxylamine  sulphate, 

50°      60°     90° 

0.522  0.560  0.685  g.  hydroxylamine  sulphate. 
(Adams,  Am.  Ch.  J.  1902,  28.  203.) 

Dry  hydroxylamine  sulphate  is  insol.  in 
abs.  and  almost  insol.  in  95%  alcohol. 
(Adams.) 

For  double  salts,  see  under  sulphuric  acid. 

NH2OH,  H2SO4.  Deliquescent.  Sol.  in 
H2O.  (Divers,  Chem.  Soc.  1895,  67.  226.) 

Hydroxylamine  tungstate,  4NH2OH,  3WO3+ 
3H2O. 

Moderately  sol.  in  H2O.  (Allen  and  Gott- 
schalk,  Am.  Ch.  J.  1902,  27.  338.) 


HYDROXYLAMINE  DISULPHONATE  SODIUM  CHLORIDE,  POTASSIUM     387 


Hydroxylamine  uranate,  UO4(NH3O)2+H2O. 
Decomp.  by  heat.     (Hofmann,  Z.  anorg. 
1897,  15.  78.) 

Hydroxylamine  uranate  ammonia, 

UO4(NH3O)2,  2NH3. 

Decomp.  by  H2O.     (Hofmann,  Z.  anorg. 
1897,  16.  79.) 


Hydroxylamine  raetavanadate,  VO6N5Hi6. 
Decomp.    by    moisture.       (Hofmann, 
anorg.  1898,  16.  472.) 


Z. 


Hydroxylamine  raetavanadate  ammonia, 

VO3H,  (NH3O)2,  2NH3. 
Easily  decomp.  by  H2O  and  HC1.     (Hof- 
mann, Z.  anorg.  1898,  16.  471.) 

Hydroxylamine  monosulphonic  acid, 
HONH(SO3H). 

"Sulphazidic  acid"  of  Fremy. 

"Sulphydroxylamic  acid"  of  Glaus. 

Sol.  in  H2O.     Slowly  decomp.  on  boiling. 
(Raschig,  A.  241.  161.) 

Ammonium  hydroxylamine  monosulphonate, 

(OH)HN,  SO3NH4. 
(Sabanejeff,  Z.  anorg.  1898,  17.  491.) 


Mowobarium  — — •  

H2O. 

Easily  sol.  in  H20. 
Chem.  Soc.  55.  760.) 


(HONHS03)2Ba+ 
( Divers  and  Haga, 

Ba(HONSO3)2Ba+ 


Dibarium    — 

H20. 

Nearly  insol.  in  H2O;  sol.  in  HCl+Aq. 
(Divers  and  Haga,  Chem.  Soc.  55.  760.) 

Pofassium ,  HONH(SO3K). 

"Potassium  sulphydroxylamate"  of  Glaus. 
"Potassium  sulphazidate"  of  Fremy. 

Sol.  in  cold  H2O.  Easily  sol.  in  hot  H?0 
without  decomp.  Insol.  in  alcohol.  (Raschig. 

+H2O.  (Divers  and  Haga,  Chem.  Soc.  55. 
760.) 

Hydroxylamine  c&sulphomc  acid, 

HON(SO3H)2. 

" Disulphydroazptic  acid"  of  Glaus. 
"Sulphazotic  acid"  of  Fremy. 
Not  known  in  free  state.    (Raschig,  A.  241. 
161.) 

Barium  hydroxylamine  disulphonate, 

Ba3(NS2O7)2+4H2O  and  +8H2O. 
Practically  insol.  in  H2O.    Sol.  in  NH4Cl-f 
Aq.    (Divers,  Chem.  Soc.  1894,  65.  559.) 

Barium  potassium . 

Ba3K8H4(NS2O7)6+9H2O. 

BaKNS2O7+H2O. 

(HO)2Ba6K4H(NS2O7)6+H2O. 


Ba9K3(NS2O7)7+14H2O. 
3Ba(OH)2,  Ba9K3(NS207)7. 
Above  salts  are  all  ppts.     (Divers,  Chem. 
Soc.  1894,  65.  561.) 

Barium  sodium  hydroxylamine  cftsulphonate, 

Ba6Na3(NS207)5+7H20. 
Ba9Na3(NS2O7)7+7H2O. 
Ba18Na15(NS2O7)17+24H2p. 
Above  salts  are  ppts.    (Divers.) 

Potassium ,  HON(SO3K)2+2H2O. 

' '  Potassium  disulphydroxy  azotate ' '  of 
Glaus  (A.  158.  75).  Insol.  in  cold  H2O. 

Very  unstable.  Very  difficultly  sol.  in  H2O, 
more  easily  in  dil.  KOH+Aq.  (Raschig,  A. 
241.  161.) 

HON(SO3K)2,  KON(SO3K)2+H2O.  True 
composition  of  potassium  sulphazotate  of 
Fremy.  (Divers  and  Haga,  Chem.  Soc.  1900, 
77.  432.) 

Potassium  sodium  — —  — — -. 

3K3NS2O7,  2Na3NS2O7+2H2O.  Sol.  in 
H2O. 

6K3NS2O7,  Na3NS2O7,  H3NS2O7+20H2O. 
Sol.  in  H2O. 

K2Na16H3(NS2O7)7+5H2O.  Less  sol.  in 
H2O  than  the  others. 

K15Na5H4(NS2O7)8+9H2O.    Sol.  in  H2O. 

KNa4H(NS2O7)2+H2O.  Readily  sol.  in 
H2O. 

K6NaH2(NS2O7)3+2H2O.  Moderately  sol. 
in  H2O. 

KNaHNS2O7-h3H2O.    Sol.  in  H2O. 
(Divers,  Chem.  Soc.  1894,  65.  552.) 

Potassium  strontium  — —  — — , 

(HO,  Sr)3NS2O7,  8(SrKNS2O7,  2H2O). 
Ppt.    (Divers.) 

Potassium  hydroxylamine  cfo'sulphonate  ni- 
trite, HON(SO3K)2,  KNO2. 

Very  si.  in  H2O.  (Divers  and  Haga, 
Chem.  Soc.  1900,  77.  433.) 

K6H(NS2O7)2,3KN02+H2O.  Decomp.  by 
H2O.  (Divers  and  Haga.) 

2KON(SQ,K)2,  KNO2+4.4H2O.  Very  sol. 
in  H2O  which  decomp.  it  into  its  constituent 
salts.  (Divers  and  Haga.) 

+6H2O.  Very  sol.  in  H2O  which  decomp. 
it  into  its  constituent  salts.  (Divers  and 
Haga.) 

2K5H(NS2O7)2,  7KNO2+3H2O.  Decomp. 
by  H2O.  (Divers  and  Haga.) 

3K5H(NS2O7)2,  7KNO2.  Decomp.  by  H2O. 
(Divers  and  Haga.) 

Potassium  hydroxylamine  disulphonate  so- 
dium   chloride,    5K2HNS2O7,    8NaCl  + 
3H2O. 
Decomp.  by  H2O.     (Divers,  Chem.  Soc. 

1894,  65.  551.) 


388 


HYDROXYLAMINE  SULPHONATE,  SODIUM 


Sodium  hydroxylamine  di'sulphonate, 

HON(SO3Na)2. 

Sol.  in  somewhat  more  than  its  own  wt.  of 
H2O  at  14°.  (Divers,  Chem.  Soc.  1894,  65. 
546.) 

Na2HNS2O7,  2Na3NS2O7+3H2O.  Sol.  in 
less  than  1.5  pts.  H2O  at  14°.  (Divers.) 

Hydroxylamine    isomonosuLphomc    acid, 

NH2,  O,  S02,  OH. 

Very  hydroscopic.  Sol.  in  water;  sol.  in 
alcohol.  (Sommer,  B.  1914,  47.  1226.) 

[Compare  Raschig,  A.  1887,  241.  161.] 

Hydroxylamine  zsocfo'sulphonic  acid. 

Ammonium  hydroxylamine  zsoc&sulphonate, 

(SO3NH4)ONH(SO3NH4). 
3  pts.  are  sol.  in  2  pts.  H2O  at  18°.    Apt 
to  form  supersat.  solutions.    (Haga,  Chem. 
Soc.  1906,  89.  246.) 

Zhpotassium ,  K2HS2O7N. 

Only  si.  sol.  in  cold  H2O.  Easily  sol.  in 
boiling  H2O.  Decomp.  by  hot  dil.  HCL 
(Raschig,  B.  1906,  39.  246.) 

6.44  pts.  are  sol.  in  100  pts.  H2O  at  16.4°. 

7.18     "     "     "    "  100    "    H20   "  17.8°. 

8.05     "    "     "    "  100    "    H2O   "  20°. 
(Haga,  Chem.  Soc.  1906,  39.  243.) 

rnpotassium ,  (SO3K)ONK(SO3K) 

+2H2O. 
Very  sol.  in  H2O;  ppt.  by  alcohol.    (Haga.) 


Disodium 


-,  (S03Na)ONH(SO3Na). 


Very  sol.  in  H2O;  insol.  in  alcohol  by  which 
it  is  ppt.  from  aqueous  solution.    (Haga.) 


Tn'sodium  — 
+2H2O. 


-,  (SO3Na)ONNa(SO3Na) 


Sol.  in  H2O;  ppt.  by  alcohol.    (Haga.) 
+3H2O.    Sol.  in  1.3  pts.  H2O  at  20°.    Less 

sol.  in   NaOH+Aq.      (Divers,   Chem.   Soc. 

1894,  65.  546.) 

Hydroxylamine  Jn'sulphonic  acid. 

Ammonium  hydroxylamine  tfn'sulphonate, 

2(SO3NH4)ON(SO3NH4)2+3H20. 
Sol.  in  0.61  pts.  H2O  at  16°.    (Haga,  Chem. 
Soc.  1904,  85.  84.) 


Potassium 
3H20. 


-,  2(S03K)ON(S03K)2  + 


1  pt.  is  sol.  in  25.37  pts.  H2O  at  18°.    (Haga.) 


Sodium  — 
2H20. 


-,   (S03Na)ON(S03Na)2+ 


Sol.  in  2.84  pts.  H2O  at  21.5°. 


Dihydroxylamine       sulphonic      acid, 

(HO)2N(S03H). 
"Sulphazinous  acid"  of  Fremy. 
Known  only  in  its  salts.    (Raschig,  A.  241. 
161.) 

Potassium      ^hydroxylamine       sulphonate, 
(HO)2NSO3K. 

Not  obtained  in  pure  state:  forms  basic  salt 
K"O 
jr^NSOsK,  which  is  quite  sol.  in  H2O,  and 

corresponds    to    "sulfazite   de   potasse"    of 
Fremy  (A.  ch.  (3)  15.  421). 

Sol.  in  H2O;  insol.  in  alohol  and  ether. 
(Fremy.) 

Hydroxyliodoplatincfo'amine  sulphate, 

(OH)IPt(NH3)4SO4+H2O. 
Very  si.  sol.,  even  in  boiling  H2O.     (Carl- 
gren,  Sv.  V.  A.  F.  47.  312.) 

Hydroxylonitratoplatin^amme    nitrate. 

OH  p,N2H6N03 

N03FtN2H6N03. 

SI.  sol.  in  cold,  more  easily  in  hot  H2O 
Very  si.  sol.  in  H2O  containing  HNO3.  (Cleve.) 

— —  pi/rophosphate, 

OH  p,N2H6    p  n    ,  TT  n 

[N03PtN2H6J2P2°7+H2°- 

Very  si.  sol.  in  H2O.    (Cleve.) 

Hydroxyloplatinamine  hydroxide, 

(OH)2Pt(NH3OH)2. 

Insol.  in  H2O.  Easily  sol.  in  dil.  acids,  even 
HC2H3O2+Aq.  Not  decomp.  by  boiling 
KOH+Aq.  (Gerhardt,  Compt.  Chem.  1849. 
490.) 

• 
Hydroxyloplatinamine  nitrate, 

(OH)2Pt(NH3NO3)2+2H2O. 
SI.  sol.  in  cold,  easily  in  hot  H20;  not 
attacked  by  cold  HCl+Aq.    (Cleve.) 


— —  oxalate,  (OH)2Pt(NH3)2C2O4+H2O. 
Sol.  in  hot  H2O. 

—  sulphate,  (OH)2Pt(NH3)2SO4+HO.2 
Difficultly  sol.  in  H2O.    (Cleve.) 

Hydroxyloplatinefo'amine  bromide, 

(OH)2Pt(NH3)4Br2. 

SI.  sol.,  even  in  boiling  H2O.     (Carleren, 
Sv.  V.  A.  F.  47.  320.) 

chloride,  (OH)2Pt(NH3)4Cl2. 

Sol.  in  206  pts.  cold,  and  49  pts.  boiling 
H2O.    (Carlgren,  Sv.  V.  A.  F.  47.  316.) 

— -  chromate,  (OH)2Pt(NH3)4Cr2O7. 

Very  si.  sol.  in  cold  or  hot  H20.    (Carlgren, 
Sv.  V.  A.  F.  47.  319.) 


HYPOBROMITE,  BARIUM 


389 


Hydroxyloplatincfaatnine  iodide, 

(OH)2Pt(NH3)J2. 
SI.  sol.  in  hot  or  cold  H2O.    (Carlgren.) 

nitrate,  (OH)2Pt(NH3)4(NO3)2. 

SI.  sol.  in  cold,  moderately  sol.  in  hot  H2O. 
(Gerhardt,  A.  76.  315.) 

Sol.  in  343  pts.  cold,  and  38  pts.  boiling 
H20.  (Carlgren,  Sv.  V.  A.  F.  47.  318.) 

—  nitrite,  (OH)2Pt(NH3)4(NO2)2. 
Easily  sol.  in  H2O.    (Carlgren.) 

sulphate,  (OH)2Pt(NH3)4SO4. 

Very  si.  sol.  in  boiling  H2O.    (Cleve.) 
+4H2O.    Efflorescent.     (Carlgren,  Sv..V. 

A.  F.  47.  313.) 

Hydroxyloplatinmcwocfa'amine  nitrate, 
,OHx  p,NH3NH3N03 

lH)2PfcNH3N03. 
Very  easily  sol.  in  H2O.    (Cleve.) 

Hydroxyloplatinsew^amine  nitrate, 

(OH)3PtNH3NH3NO3(?). 
Easily  sol.  in  U2O.    (Cleve.) 

sulphate, 

(OH)2PtNH3NH3 
W        (?). 
S04 
Sol.  in  hot  H2O. 

Hydroxylocfo'platincfo'amine  chloride, 

(OH)2Pt2(NaH6)4Cl4+H20. 
Extremely  si.  sol.  in  H2O. 

cftchromate,  (OH)2Pt2(N2H6)4(Cr2O7)2. 

Ppt.    (Cleve.) 

nitrate,  (OH)2Pt2(N2H6)4(NO3)4. 

Very  si.  sol.  in  cold,  more  easily  in  hot  H2O. 
(Cleve.) 

phosphate,  (OH)2Pt2(N2H6)4(PO4H)2. 

Ppt. 

sulphate,  (OH)2Pt2(N2H6)4(S04)2+ 

2H2O. 
Ppt.    Nearly  insol.  in  H2O. 

Hydroxylosulphatoplatindi'amine 
bromide,  (OH)Pt(N2H6)2Br. 

\  /       +2H20. 
SO, 
Easily  sol.  in  H2O.    (Cleve.) 

(OH)PUN2H6)2C1 

chloride,  \   /        +2H2O. 

SO4 

Moderately  sol.  in  cold,  very  sol.  in  hot 
H2O. 


Hydroxylosulphatoplatinc^amine    chloroplati- 
nate, 

r(OH)Pt(N2H6)2Cl-i 
2  \/  ,  PtCl4+2H2O. 

L  S04        -I 

Ppt. 

chromate, 

r(OH)Pt(N2H6)2-i 

\/        Cr04+2H20. 
S04     -12 
SI.  sol.  in  H2O. 


r(OH)Pt(N2H6)2- 
bichromate,  \  /       |  Cr2O7. 

.81.  sol.  inH2O. 


S04 


(OH)Pt(N2H6)2N03. 

nitrate,  \  / 

S04 
Sol.  in  hot  H2O. 

sulphate, 

r(OH)Pt(N2HG)2-i 

\/        S04+3H2(X 
S04      -J2 
SI.  sol.  in  H20.    (Cleve.) 

Hypoantimonic  acid. 

Calcium  hypoantimonate  (?),  Ca2Sb3O8. 
Min.  Romeite.    Insol.  in  acids. 

Potassium  hypoantimonate,  K2Sb2O5. 

Sol.  in  hot  H2O.  Sol.  in  425  pts.  boiling 
H2O  (Brandes).  Sol.  in  boiling  KOH+Aq 
(Berzelius). 

K2Sb4O9.    Ppt. 

Hypoboric  acid. 

Sodium  hypoborate,  NaOBH3. 

Deliquescent,  decomp.  in  aq.  solution  at 
room  temp.  Decomp.  by  acids.  SI.  sol.  in 
alcohol  with  decomp.  (Stock,  B.  1914,  47. 
821.) 

Hypobromous  acid,  HBrO. 

Known  only  in  aqueous  solution. 

Solution  containing  6.21  pts.  Br  as  HBrO 
in  100  com.  H2O  decomposes  at  30°.  If  dilute 
solution  is  distilled  in  vacuo,  an  acid  contain- 
ing 0.736  pt.  Br  as  HBrO  in  100  ccm.  is  ob- 
tained at  first,  but  tfie  distillate  slowly  grows 
weaker.  Dil.  solution,  stable  at  ordinary 
temp.,  decomp.  bv  heating  over  60°.  (Dancer 
A.  125.  237.) 

Barium  hypobromite. 
Known  only  in  solution. 


390 


HYPOBROMITE  BROMIDE,  CALCIUM 


Calcium  hypobromite  bromide. 

Deliquescent,  and  sol.  in  H2O  with  partial 
decomp.  (Berzelius.) 

Potassium  hypobromite,  KBrO. 
Known  only  in  solution. 

Sodium  hypobromite. 
Known  only  in  solution. 

Strontium  hypobromite. 
Known  only  in  solution. 

Hypochlorous  acid,  HC1O. 

Miscible  with  H2O.  Decomposes  at  0°  in 
the  dark,  more  rapidly  at  higher  temp,  or  in 
light.  The  stronger  the  solution  the  more 
rapid  the  decomposition.  Moderately  strong 
acid  may  be  distilled  without  any  consider- 
able decomp.,  a  stronger  acid  distilling  over 
at  first,  and  afterwards  an  acid  weaker  than 
the  original  acid.  Very  cone,  or  very  dil. 
acids  decomp.  by  distillation. 

Ammonium  hypochlorite. 

Known  only  in  aqueous  solution,  which  de- 
composes at  once. 

Barium  hypochlorite. 
Known  only  in  solution. 

Calcium  hypochlorite,  Ca(OCl)2+4H2O. 

Deliquescent,  and  sol.  in  H2O.  (Kinzgett, 
Chem.  Soc.  (2)  13.  404.) 

Calcium  hypochlorite  chloride,  etc.  (bleaching 
powder),  Ca(OCl)2,  CaCl2,  Ca(OH)2+ 
H2O. 

Not  deliquescent.  Sol.  in  H2O.  Alcohol 
does  not  dissolve  out  CaCl2.  Sol.  in  20  pts. 
H2O  with  a  slight  residue. 

Correct   formula  is   CaOCl2    (Lunge   and 

Schappi;  Kraut,  A.  214.  354),  Ca^1  (Stahl- 
schmidt,  B.  8.  869),  CaOCl,  Cl  (Odling). 

CaCl2  is  dissolved  out  by  alcohol.  For- 
mula =2Ca^1CaCl+2H2O.  (Dreyfuss,  Bull. 
Soc.  (2)  41.  600.) 

Didymium  hypochlorite,  Di(OCl)3. 

Difficultly  sol.  in  H2O.  Easily  sol.  in  acids. 
(Frerichs  and  Smith,  A.  191.  348.) 

Lanthanum  hypochlorite,  La(OCl)3. 

Easily  sol.  in  H2O.    (Frerichs  and  Smith.) 

Lithium  hypochlorite,  LiClO. 

Known  only  in  solution.  (Kraut,  A.  1882, 
214.  356.) 

Magnesium  hypochlorite. 
Known  only  in  solution. 


Potassium  hypochlorite,  KC1O. 
Known  only  in  solution. 

Silver  hypochlorite,  AgClO. 

Very  sol.  in  H2O,  and  decomp.  very  quickly. 
(Stas,  Acad.  R.  de  Belg.  35.  103.) 

Sodium  hypochlorite,  NaClO. 
Known  only  in  solution. 

Hypoiodic  acid,  I2O4. 
See  Iodine  textroxide. 

Hypoiodous  acid,  HOI. 

Known  only  in  solution  which  decomp.  on 
standing.  (Taylor,  C.  N.  1897,  76.  97.) 

Calcium  hypoiodite  iodide,  Ca(OI)2,  CaI2. 

Not  very  unstable.  (Lunge  and  Shoch,  B. 
16.  1883.) 

Hyponitric  acid,  N2O4. 
See  Nitrogen  tetroxide. 

Hyponitrous  acid,  HNO,  or  better  H2N2O2. 

Known  only  in  aqueous  solution.  Solution 
is  quite  stable,  (van  der  Plaats,  B.  10.  1507.) 

Very  deliquescent;  sol.  in  H2O  and  alcohol; 
sol.  in  ether,  chloroform,  benzene;  si.  sol.  in 
petroleum  ether.  (Hantzsch  and  Kaufmann, 
A.  1896,  292.  323.) 

Ammonium  hyponitrite,  (NH4)2N2O2. 

Sol.  in  H2O  and  in  alcohol.  (Jackson,  C.  N. 
1893,  68.  266.) 

Ammonium  hydrogen  hyponitrite,  NH4HN202 
Easily  sol.  in  H2O.  The  solid  salt  slowly 
decomp.  at  ord.  temp,  into  ammonia,  H2O 
and  N2O.  (Hantzsch  and  Kaufmann,  A. 
1896,  292.  328.) 

Barium  hyponitrite,  BaN2O2. 

Nearly  insol.  in,  but  gradually  decomp.  by 
H2O.  Sol.  in  cone,  acids  with"  evolution  of 
N2O,  but  sol.  in  dil.  HC2H3O2+Aq  without 
decomp.  (Zorn,  B.  16.  1007.) 

+4H2O.  SI.  sol.  in  H2O;  insol.  in  alcohol 
and  ether.  (Kirschner,  Z.  anorg.  1898,  16. 
424.) 

+zH2O.  Efflorescent.  (Maquenne,  C.  R. 
108.  1303.) 

Barium  hydrogen  hyponitrite,  BaH2(N2O2)2. 

Easily  sol.  in  H2O.  (Zorn,  B.  1882,  16. 
1011.) 

Calcium  hyponitrite,  CaN2O2+ 4H2O. 

Nearly  insol.  in  H2O;  easily  sol.  in  dil. 
acids.  (Maquenne,  C.  R.  108.  1303.) 

SI.  sol.  in  H2O;  insol.  in  alcohol.  (Kirsch- 
ner, Z.  anorg.  1898,  16.  426.) 


HYPOPHOSPHATE,  BARIUM  HYDROGEN 


391 


Cupric  hyponitrite,  basic,  CuN2O2,  Cu(OH)2. 

Insol.  in  H2O;  not  decomp.  by  hot  H2O. 
Sol.  in  dil.  acids  and  in  ammonia.  Decomp. 
by  NaOH.  (Divers,  Chem.  Spc.  1899,  76. 121 . 

Insol.  in  H2O.  Sol.  in  dil.  acids  and  in 
NH4OH+Aq.  (Kirschner,  Z.  anorg.  1898, 
16.  430.) 

Cuprous  hyponitrite,  Cu2N2O2+2H2O. 
Ppt.    (Kolotow,  C.  C.  1891,  I.  1859.) 
Cannot  be  formed.     (Divers,  Chem.  Soc. 

1899,  75.  121.) 

Lead  hyponitrite,  basic,  PbN2O2,  PbO. 

Insol.  in  H2O.  Sol.  in  dil.  acids  from  which 
it  may  be  pptd.  by  NaOH+Aq  or  NH4OH  + 
Aq.  (Kirschner,  Z.  anorg.  1898,  16.  430.) 

Lead  hyponitrite,  PbN2O2. 

Insol.  in  H2O;  sol.  in  dil.  acids  from  which 
it  may  be  pptd.  by  NaOH+Aq  or  NH3+Aq. 
(Kirschner.) 

Mercuric  hyponitrite,  basic,  3HgO,  HgN2O2 

+3H20. 

Ppt.  SI.  sol.  even  in  boiling  dil.  HNO3. 
Scarcely  sol.  in  cone.,  very  sol.  in  warm  dil. 
HC1.  (Ray,  Chem.  Soc.  1897,  71.  349.) 

Mercurous  hyponitrite,  Hg2N2O2. 

Sol.  in  dil.  HNO3  with  slow  decomp.  (Ray, 
Chem.  Soc.  1907,  91.  1404.) 

Mercuric  hyponitrite,  HgN2O2. 

Sol.  in  HC1,  and  in  NaCl+Aq. 

SI.  sol.  in  very  dil.  alkali.  (Divers,  Chem. 
Soc.  1899,  75.  119.)  . 

Potassium  hyponitrite,  K2N2O2. 

Sol.  in  H20.    (van  der  Plaats.) 

Stable  when  dry. 

Sol.  in  90%  alcohol,  and  si.  sol.  in  abs. 
alcohol.  (Divers,  Chem.  Soc.  1899,  75.  103.) 

Silver  hyponitrite  (nitrosyl  silver), 
Ag2N2O2. 

Insol.  in  H2O.  Easily  sol.  in  dil.  HNO3+ 
Aq  or  H2SO4+Aq. 

Decomp.  by  H3P04,  H2S,  and  boiling 
HC2H3O2+Aq.  (van  der  Plaats.) 

Insol.  in  HC2H3O2+Aa;  sol.  in  NH4OH 
+Aq.  (Divers,  C.  N.  23.  206.) 

Sol.  in  dil.  HNO3  and  H2SO4  and  in  cone. 
NH4OH+Aq;  decomp.  by  HC1.  (Kirsch- 
ner, Z.  anorg.  1898,  16.  431.) 

Sodium  hyponitrite,  Na2N2O2+6H2O. 
Sol.  in  H2O.    (van  der  Plaats.) 

Strontium  hyponitrite,  SrN2O2. 

Easily  sol.  in  H2O.  (Roederer,  Bull. 
Soc.  1906,  (3)  35.  715.) 

+5H2O.    Nearly  insol.  in  H2O;  easily  sol. 


in  dil.  acids.    (Maquenne,  C.  R.  108.  1303.) 
SI.  sol.  in  H2O,  insol  in  alcohol.    (Kirsch- 
ner, Z.  anorg.  1898,  16.  426.) 

Hypophosphomolybdic  acid,  Mo5O8, 

7H3PO2+3H2O. 

Very  si.  sol.  in  cold  H2O.  Scarcely  sol. 
in  cold  dil.  H2SO4.  Sol.  in  cold  cone.  H2SO4. 
Sol.  in  warm  cone.  HC1.  Warm  HNO, 
oxidizes  forming  clear  solution.  (Mawrow, 
Z.  anorg.  1901,  28.  164.) 

Ammonium  hypophosphomolybdate, 

2(NH4)2O,  2H3PO2,  8MoO3+2H2O. 
Not  very  sol.  in  cold  H2O,  readily  in  hot 
H2O.    (Gibbs,  Am.  Ch.  J.  3.  402.) 

Hypophosphoric  acid,  H4P2O6. 

Very  deliquescent,  and  sol.  in  the  least 
amount  of  H2O.  (Joly,  C.  R.  101.  1058.) 

100  cc.  H4P2O6+Aq,  containing  4.1%P2O4 
has  sp.  gr.  =  1.036. 

100  cc.  H4P2O6-t-Aq,  containing  12.3% 
P2O4hassp.  gr.  =  1.122. 

(Salzer,  A.  1878,  194.  28.) 

+H2O.    (Sanger,  A.  232. 14.) 

Does  not  exist.    (Joly.) 

+2H2O.  Appears  to  be  the  only  stable 
hydrate  between  0°  and  60.° 

Sanger's  hydrate,  H4P2O6+H2O,  and 
Joly's  anhydride  could  not  be  obtained. 
(Rosenheim,  B.  1908,  41.  2711.) 

Aluminum    hypophosphate,    A14  ( P2O6)  3  + 

23H20.    " 

Easily  sol.  in  mineral  acids.  Sol.  in  Na4P206 
+Aq.  (Palm,  Dissertation,  Rostock,  1890.) 

Ammonium    hypophosphate,     (NH4)4P206+ 

H20. 
Sol.  in  30  pts.  H2O.    (Salzer,  A.  194.  32.) 

Ammonium  hydrogen  hypophosphate, 

(NH4)2H2P206. 

Sol.  in  14  pts.  cold,  and  4  pts.  boiling  H2O. 
(Salzer,  A.  194.  32.) 

Ammonium  frzhydrogen  hypophosphate, 

NH4H3P206; 
Sol.inH2O.    (Salzer,  A.  211. 1.) 

Ammonium  magnesium  hypophosphate, 

(NH4)2MgP206+6H20. 
Precipitate.     (Salzer,  A.  232.  114.) 

Barium  hypophosphate,  Ba2P2O6. 

Very  slightly  sol.,  but  not  wholly  insol.  in 
H2O.  Very  slightly  sol.  in  acetic  acid,  but 
more  soluble  in  hydrochloric,  and  hypophoa- 
phoric  acids.  (Salzer,  A.  194.  34.) 

Barium  hydrogen  hypophosphate,  BaH2P2O6 

+2H20. 

Soluble  in  about  1000  pts.  H2O.  Solution 
decomposes  by  heating.  (Salzer,  A.  194.  34.) 


392 


HYPOPHOSPHATE,  BISMUTH 


Bismuth     hypophosphate,     Bi4(P2O6)3  + 


Completely  sol.  in  HCl+Aq,  also  in  warm 
HNOg+Aq.  Insol.  in  boiling  dil.  H2SO4+ 
Aq.  SI.  sol.  by  long  boiling  with  cone. 
H2SO4.  (Palm,  Rostock,  1890.) 

Cadmium  hypophosphate,  Cd2P2O6+2H2O. 

Insol.  in  H2O.  Sol.  in  dil.  acids.  (Drawe, 
B.  21.  3403.) 

Cadmium    potassium    hydrogen    hypophos- 
phate, CdK2(H2P206)2+2^H2O. 
(Bausa,  Z.  anorg.  1894,  6.  147.) 

Cadmium  sodium  hypophosphate,  CdNa2P2O6 

+6H2O. 

Insol.  in  H2O,  but  decomp.  thereby.  Sol. 
in  dil.  acids.  (Drawe.) 

Calcium  hypophosphate,   Ca2P2O6+2H2O. 

Insol.  in  H2O;  difficultly  sol.  in  HC2H3O2; 
easily  sol.  in  H4P2O6,  or  HCl+Aq.  (Salzer, 

A.  194.  36.) 

Calcium  hydrogen  hypophosphate, 

CaH2P2O6+  6H2O. 
Sol.  in  60  pts.  H2O.    (Salzer,  A.  232.  114.) 

Chromic  hypophosphate,  Cr4(P2O6)?+34H2O. 
Sol.  in  HCl+Aq  on  si.  warming,  also  in 
HNO3+Aq.  Not  completely  sol.  in  dil. 
H2SO4+Aq,  but  completely  sol.  in  cone. 
H2SO4.  (Palm,  Dissertation,  Rostock,  1890.) 

Cobaltous  hypophosphate,  Co2P2O6+8H2O. 
Insol.  in  H2O.   Easily  sol.  in  acids.    (Drawe, 

B.  21.  3403.) 

Cobaltous  potassium  hypophosphate, 

CoK2P206+5H20. 
Ppt.    (Bausa,  Z.  anorg.  1894,  6.  156.) 

Cobaltous    potassium    hydrogen    hypophos- 
phate, CoH2P2O6,  3K2H2P2O6+15H2O. 

Cobaltous  sodium  hypophosphate,  CoNa2P2O6 

Insol.  in  H2O,  but  decomp.  thereby.  Sol. 
in  dil.  acids.  (Drawe,  B.  21.  3403.) 

Cupric  hypophosphate,  Cu2P2O6+6H2O. 

Insol.  in  H2O.  Sol.  in  dil.  acids.  (Drawe, 
B.  21.  3403.) 

Ppt.    (Bausa,  Z.  anorg.  1894,  6.  145.) 

Cupric  potassium  hydrogen  hypophosphate, 

CuH2P2O6,  3K2H2P2O6+15H2O. 
Ppt.    (Bausa,  Z.  anorg.  1894,  6.  152.) 

Glucinum  hypophosphate,  G12P2O6+7H2O. 

Insol.  in  H2O.  Moderately  sol.  in  all  min- 
eral acids.  (Palm,  Rostock,  1890.) 

+3H2O.     (Rammelsberg.) 


Iron     (ferrous)    hypophosphate,    Fe2P206 


Insol.  in  H2O.  Sol.  in  cold  HCl+Aq. 
Decomp.  by  hot  HNO3+Aq  into  Fe4(P2O6)3. 
Insol.  in  HNO3+Aq.  Insol.  in  boiling  dil. 
H2SO4+Aq.  Somewhat  sol.  in  cold  H2SO4, 
but  a  ppt.  separates  out  on  heating.  (Palm, 
Rostock,  1890.) 

Iron    (ferric)    hypophosphate,    Fe4(P2O6)3+ 

20H2O. 

Easily  sot.  in  HCl+Aq.  Wholly  insol.  in 
HNO3,  and  dil.  H2SO4+Aq.  Completely  sol. 
in  cone.  H2SO4  by  warming  a  short  time,  but  a 
ppt.  separates  out  on  boiling.  (Palm.) 

Lead  hypophosphate,  Pb2P206. 

Insol.  in  H2O,  HC2H3O2,  or  H4P2O6+Aq; 
sol.  in  dil.  HN03+Aq.  (Salzer.) 

Lithium  hypophosphate,  Li4P2O6+7H2O. 
Very  si.  sol.  in  H2O.    (Salzer,  A.  194.  28.) 
Sol.  in  120  pts.  H2O  at  ord.  temp.    (Ram- 

melsberg, J.  pr.  (2)  45.  153.) 

Li2H2P2O6+2H2O.     Deliquescent.     (Ram- 

melsberg.) 

Magnesium    hypophosphate,    Mg2P2O6  + 
12H2O. 

Sol.  in  15,000  pts.  H2O;  si.  sol.  in  acetic, 
easily  in  hypophosphoric,  or  mineral  acids. 
(Salzer,  A.  232.  114.) 

+24H2O.    (Rammelsberg.) 

Magnesium  hydrogen  hypophosphate, 

MgH2P2O6+4H2O. 
Sol.  in  200  pts.  H20.    (Salzer,  A.  232.  114.) 

Manganese    hypophosphate,    Mn2P2O6  + 


Insol.  in  H20;  sol.  in  mineral  acids,  insol. 
in  acetic  acid.  (Palm,  Dissertation,  Rostock, 
1890.) 

Manganous  potassium  hydrogen  hypophos- 

phate, MnH2P2O6,  K2H2P2O6+3H2O. 
Ppt.    (Bausa,  Z.  anorg.  1894,  6.  150.) 

Manganous  sodium  hypophosphate,  Mn2P2O6, 

Na4P2O6+llH2O. 
Insol.  in  H2O;  sol.  in  mineral  acids.    (Palm.) 

Nickel  hypophosphate,  Ni2P2O6  +  12H2O. 

Insol.  in  H2O.  Sol.  in  dil.  acids.  (Drawe, 
B.  21.  3401.) 

Nickel  potassium  hypophosphate, 

NiK2P2O6+6H2O. 
Ppt.    (Bausa,  Z.  anorg.  1894,  6.  155.) 

Nickel  potassium  hydrogen  hypophosphate, 

NiH2P2O6,  3K2H2P2O6+15H2O. 
Ppt.    (Bausa,  Z.  anorg.  1894,  6.  144.) 


HYPOPHOSPHITE,  CEROUS 


393 


Nickel  sodium  hypophosphate,  NiNa2P2O6+ 

12H2O. 

Insol.  in  H2O,  but  decomp.  thereby.  Easily 
sol.  in  dil.  acids.  (Drawe.) 

Potassium  hypophosphate,  K4P2O6+8H2O. 
Sol.  in   M  pt.  H2O;  insol.  in  alcohol. 
(Salzer,  A.  211.  1.) 

Potassium   hydrogen   hypophosphate. 

K3HP206+3H20. 
Sol.  in  Y2  pt.  H2O.    (Salzer,  A.  211. 1.) 

Potassium  dihydrogen  hypophosphate, 

K2H2P2O6+3H2O,  and  +2H2O. 
Sol.  in  3  pts.  cold,  and  1  pt.  boiling  H2O. 
(Salzer,  A.  211.  1.) 

Potassium  ^n'hydrogen  hypophosphate, 

KH3P2O6. 

Sol.  in  \Y2  pts.  cold,  and  ^  pt.  hot  H2O. 
(Salzer,  A.  211.  1.) 

Potassium  pentohydrogen  cfahypophosphate, 

K3H5(P206)2+2H20. 

Sol.  in  21A  pts.  cold,  and  %  pt.  boiling 
H2O.  (Salzer,  A.  211.  1.) 

Potassium  sodium  hypophosphate, 

Na2K2P206+9H20. 

Sol.  in  about  25  pts.  cold,  and  3  pts.  hot 
H2O.  (Bausa,  Z.  anorg.  1894,  6.  158.) 

Potassium  zinc  hydrogen  hypophosphate, 

ZnH2P2O6,  3K2H2P2O6  +  15H2O. 
Ppt.    (Bausa,  Z.  anorg.  1894,  6.  148.) 

Silver  hypophosphate,  Ag4P2O6. 

SI.  sol.  in  H2O.  Easily  sol.  in  HNO3,  or 
NH4OH+Aq.  Very  si.  sol.  in  H4P2O6+Aq. 
(Salzer,  A.  232.  114.) 

Sodium  hypophosphate,  Na4P2O6+10H2O. 

Sol.  in  about  30  pts.  cold,  much  more  easily 
in  hot  H2O.  (Salzer.) 

Sodium  hydrogen  hypophosphate,  Na3HP2O6 
+9H2O. 

Sol.  in  22  pts.  H2O.    (Salzer.) 

Sodium  ^hydrogen  hypophosphate, 

Na2H2P2O6+6H2O. 

Sol.  in  45  pts.  cold,  and  5  pts.  boiling  H2O. 
More  sol.  in  dil.  H2SO4+Aq.  Insol.  in  alco- 
hol. (Salzer,  A.  187.  331.) 

Sodium  Znliydrogen  hypophosphate, 

NaH3P2O6. 
Sol.  in  H2O.    (Salzer,  A.  211.  1.) 

Sodium  ^nhydrogen  cfoliypophosphate, 

Very  efflorescent.  Sol.  in  15  pts.  cold  H2O. 
(Salzer,  A.  211.  1.) 


Thallium  hypophosphate,  T14P2O6. 

SI.  sol.  in  H2O.  Decomp.  in  sunlight. 
(Joly,  G.  R.  1894,  118.650.) 

Thallium  hydrogen  hypophosphate, 

T12H2P206. 
Sol.  in  H2O.     (Joly.) 

Zinc  hypophosphate,  Zn2P2O6+2H2O. 

Insol.  in  H2O.  Easily  sol.  in  dil.  acids. 
(Drawe,  B.  21.  3403.) 

Hypophosphorosomolybidc  acid. 

Barium  hypophosphorosomolybdate, 
BaO,  Mo7O20,  3H3PO2+12H2O. 
Very  sol.  in  H2O  and  BaCl2+Aq.    CMaw- 
row,  Z.  anorg.  1902,  29.  156.) 

Hypophosphorous  acid,  H3P02. 

Very  sol.  in  H2O  and  alcohol.    (Rose.) 

Aluminum  hypophosphite. 

Not  deliquescent,  but  very  sol.  in  H2O. 
(Rose,  Pogg.  12.  86.) 

Ammonium  hypophosphite,  NH4H2PO2. 

Sol.  in  H2O,  less  deliquescent  than  the 
potassium  salt.  (Wurtz,  A.  ch.  (3)  7.  193.) 

Very  sol.  in  absolute  alcohol.     (Dulong.) 

Moderately  sol.  in  liquid  NH3.  (Frank- 
lin, Am.  Ch.  J.  1898,  20.  826.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4328.) 

Barium  hypophosphite,  Ba(H2PO2)2+H2O. 

Sol.  in  3.5  pts.  cold,  and  3  pts.  boiling  H2O. 
Insol.  in  alcohol.  (Wurtz,  A.  43.  323.) 

Bismuth*  hypophosphite,  Bi(H2PO2)3. 
Ppt.    (Vanino,  J.  pr.  1906,  (2)  74.  150.) 
+H2O.       Sol.     in     acid     Bi(NO3)3+Aq. 

(Haga,  Chem.  Soc.  1895,  67.  229.) 

Cadmium  hypophosphite. 
Sol.  in  H2O.    (Rose,  Pogg.  12.  91.) 

Calcium  hypophosphite,  Ca(PH202)2. 

Sol.  in  6  pts.  cold,  and  not  much  more  sol. 
in  hot  H2O.  Insol.  in  strong,  very  sol.  in 
weak  alcohol.  (Rose,  Pogg.  9.  361.) 

Calcium  cobaltous  hypophosphite. 

2Ca(PH2O2)2,  Co(PH2O2)2+2H2O. 
Efflorescent.    (Rose,  Pogg.  12.  295.) 

Calcium  ferrous  hypophosphite. 
Sol.  in  H2O.    (Rose,  Pogg.  12.  294.) 

Cerous  hypophosphite,  Ce(PH2O2)3+H2O. 

SI.  sol.  in  H2O.  (Rammelsberg,  B.  A.  B. 
1872.  437.) 


394 


HYPOPHOSPHITE,  CHROMIUM 


Chromium  hypophosphite,  Cr2(OH)2(H2PO2)4. 

Anhydrous.     Insol.  in  H2O  or  dil.  acids. 

+3H2O.  Sol.  in  H2O.  (Wurtz,  A;  ch.  (3) 
16.  196.) 

Cobaltous    hypophosphite,     Co(PH2O2)2  + 
6H2O. 

Efflorescent.  Easily  sol.  in  H2O.  (Rose. 
Pogg.  12.  87.) 

Cupric  hypophosphite,  Cu(PH2O2)2. 

Very  sol.  in  H2O,  but  very  easily  decomp. 
on  heating.  (Wurtz,  A.  ch.  (3)  16.  199.) 

Glucinum  hypophosphite. 

Sol/  in  H2O.     (Rose,  Pogg.  12.  86.) 

Iron  (ferrous)  hypophosphite,  Fe(PH2O2)2-f 

6H2O. 
Sol.  in  H2O.     (Rose,  Pogg.  12.  294.) 

Iron  (ferric)  hypophosphite. 

Difficultly  sol.  in  H2O  or  acids.  Decomp. 
on  boiling.  SI.  sol.  in  H3PO2+Aq.  (Rose.) 

Lead  hypophosphite,  Pb(PH2O2)2. 

Difficultly  sol.  in  cold,  more  easily  in  hot 
H2O.  Insol.  in  alcohol.  (Rose,  Pogg.  12. 
288.) 

Lithium  hypophosphite,  LiH2PO2+H2O. 

Sol.  in  H20.  (Rammelsberg,  B.  A.  B. 
1872.  416.) 

Magnesium    hypophosphite,    Mg(PH2O2)2  + 
6H2O. 

Efflorescent  in  dry  air.     Sol.  in  H2O. 
(Rose.) 


ous    hypophosphite,    Mn(H2PO2)2  + 


M 


Permanent.     Very  sol.  in  H2O.     (Wurtz. 
A.  ch.  (3)  16.  195.) 

Mercurous  hypophosphite  nitrate, 

HgH2P02,  HgN03+H20. 
SI.  sol.  in  H20  with  rapid  decomp. 


Sol.  in  hot  cone. 
Soc.  1895,  67.  227.) 


(Haga,  Chem. 


Nickel    hypophosphite,    Ni(PH2O2)2+6H2O. 
Efflorescent.     Sol.    in   H2O.      (Rammels- 
berg, B.  5.  494.) 

Nickel  hypophosphite  ammonia, 

Ni(H2P02)2,  6NH3. 
(Ephraim,  B.  1913,  46.  3111.) 

Platinous  hypophosphite  Pt(PH2O2)2. 

Insol.  in  H2O,  HC1,  H2SO4+Aq,  etc.  Sol. 
in  HNO3-fAq.  Insol.  in  alcohol.  (Engel, 
C.  R.  91.  1068.) 


Potassium  hypophosphite,  KH2PO2. 

Very  deliquescent.  Very  sol.  in  H2O. 
sol.  in  weak,  less  in  absolute  alcohol.  Insol. 
in  ether.  (Wurtz,  A.  ch.  (3)  7.  192.) 

SI.  sol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

Sodium  hypophosphite,  NaH2PO2+H2O. 

Very  deliquescent.  Somewhat  less  sol.  than 
the  K  salt.  Very  sol.  in  absolute  alcohol. 
(Dulong.) 

Very  sol.  in  H2O,  and  somewhat  less  sol.  in 
alcohol.  (Rammelsberg,  B.  A.  B.  1872.  412.) 

SI.  sol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Strontium  hypophosphite,  Sr(PH2O2)2. 
Very  easily  sol.  in  H2O.    (Dulong.) 
Insol.  in  alcohol.     (Wurtz.) 

Thallous  hypophosphite,   T1H2PO2. 

Sol.  in  H2O.  (Rammelsberg,  B.  A.  B. 
1872.  492.) 

Uranyl  hypophosphite,  UO2(H2PO2)2+H2O. 
SI.  sol.  in  H2O.  Easily  sol.  in  HC1,  or 
HNO3+Aq.  (Rammelsberg,  Chem.  Soc. 
(2)  11.  1.) 

ZHvanadyl  hypophosphite,  V2O2(H2PO2)4-h 
2H2O. 

Insol.  in  cold,  si.  sol.  in  hot  H2O. 

Sol.  in  hot  dil.  HC1,  H2SO4  and  HNO3  and 
in  warm  cone.  HC1  and  H2SO4. 

Insol.  in  oxalic  acid.  (Mawrow,  Z.  anorg. 
1907,  65.  147.) 

Zinc  hypophosphite,  Zn(H2PO2)2+H2O. 

Sol.  in  H2O. 

+6H2O.  Efflorescent.  (Wurtz.  A.  ch.  (3) 
16.  195.) 

Zirconium  hypophosphite,  Zr(OPH2O)4+H2O. 
Sensitive  to  light.  Insol.  in  alcohol,  by 
which  it  is  pptd.  from  aqueous  solution. 
(Hauser,  Z.  anorg.  1913,  84.  93.) 

Hypophosphotungstic  acid.    * 

Potassium    hypophosphotungstate,    4K2O, 

6H3PO2,  18WO3+7H2O. 
Precipitate.     Sol.  in  hot,  very  si.  sol.  in 
cold  H2O.    (Gibbs,  Am.  Ch.  J.  5.  361.) 

Hyposulpharsenious  acid. 

Hyposulpharsenites,  As2S2,  M2S. 
Difficultly  sol.  in  H2O.     (Berzelius.) 
Do  not  exist.    (Nilson,  B.  4.  989.) 

Hypo  sulphuric  acid,  H2S2O6. 
See  Dithionic  acid. 


IMIDOPHOSPHATE,  BARIUM,  BASIC 


395 


Hyposulphurous  acid,  H2S2O3. 
See  Thiosulphuric  acid. 

Hyposulphurous  (Hydro sulphurous)  acid, 

H2SO2. 

Known  only  in  dil.  aqueous  solution, 
which  decomposes  rapidly. 

Correct  formula  is  H2S2O4,  according  to 
Bernthsen  (A.  211.  285.) 

More  sol.  in  alcohol  than  in  H2O.  (Rossler, 
Arch.  Pharm.  (3)  25.  845.) 

Ammonium  hyposulphite,  (NH4)2S2O4. 

Known  only  in  solution.  (Prudhomme, 
Bull.  Soc.  1899,  (3)  21.  326.) 

Ammonium  hydrogen  hyposulphite, 

NH4HS204. 

Known  only  in  solution.  (Prudhomme, 
Bull.  Soc.  1899,  (3)  21.  326.) 

Calcium  hyposulphite,  CaS2O4+1.5H2O. 

Difficultly  sol.  in  H2O.  (Bazlen,  B.  1905, 
38.1059.) 

Magnesium  hyposulphite,  MgS2O4. 
(Billy,  C.  R.  1905,  140.  936.) 

Potassium  hyposulphite,  K2S2O4+3H2O. 

Easily  decomp. 

Insol.  in  alcohol.  (Bazlen,  B.  1905,  38. 
1058.) 

Sodium  hyposulphite,  Na2S2O4. 

Anhydrous.  Stable  in  dry  air.  (Bazlen, 
B.  1905,  38.  1081.) 

100  g.  H2O  dissolve  24.1  g.  of  the  anhydrous 
salt  at  20°.    (Jellinek,  Z.  anorg.  1911,  70. 130.) 
+2H2O.    Solubility  in  H2O. 

11.6  g.  of  the  solution  contain  at: 
20°  1.91g.  Na2S2O4 

10°  1.67  g.   •  " 

1°  1.49g.  " 

(Jellinek,  Z.  anorg.  1911,  70.  128.) 
Insol.  in  alcohol.     (Bazlen,  B.   1905,  38. 
1058.) 

Sodium  zinc  hyposulphite,  Na2S2O4,  ZnS2O4. 
Less  sol.  in  H2O  than  ZnS2O4.     (Bazlen, 
B.  1905,  38. 1060.) 

Strontium  hyposulphite,  SrS2O4. 

Sol.  in  H2O.  (Moissan,  C.  R.  1902,  136. 
653.) 

Zinc  hyposulphite,  ZnS2O4. 

Easily  sol.  in  H2O;  about  1  pt.  in  7  pts. 
H2O.  Forms  supersat.  solutions  readily. 
(Bazlen,  B.  1905,  38.  1060.) 

Hypovanadic  acid,  V2O2(OH)4. 
See  Vanadium  tetrhy  dioxide. 


Hypovanadic  acid,  H2V4O9. 
See  Vanadous  acid. 

Hypovanadic  acid  with  vanadic  acid. 
See  Vanadicovanadic  acid. 

Imidocfa'metaarsenic  acid. 

Ammonium  imidocfo'metaaresenate, 

(NH4O2As2O3NH. 

(Rosenheim    and    Jacobsohn,    Z.    anorg. 
1908,  60.  307.) 

Imidochromic  acid. 

Ammonium  imidochromate,  ,. 

NHCrO(ONH4)2. 

Very  sol.  in  H2O  with  decomp.     (Rosen- 
heim and  Jacobsohn,  Z.  anorg.  1906,  50.  299.) 

Ammonium  potassium  imidochromate, 

NH4KCrO3NH. 

Decomp.   on   solution  in   H2O.      (Rosen- 
heim, Z.  anorg.  1906,  50.  302.) 

Imidocfo'imidcchromic  acid. 

Ammonium  imidoc&imido  chromate, 

NH[CrO(NH)ONH4]2. 
.(Rosenheim    and    Jacobsohn,    Z.    anorg 
.1906,  60.  303.) 

Imidomolybdic  acid. 

Potassium  imidomolybdate,  NKMoO(OK)2. 

Unstable  in  air. 

Very    hygroscopic.      Very    sol.    in    H2O. 
(Rosenheim,  Z.  anorg.  1906,  50.  305.) 

Dzimido^'phosphormonamic  acid, 

HO— PO  <^H>  p°— NH2- 

Correct   formula   for   p?/r0phospho£namic 
acid  of  Gladstone.    (Mente,  A.  248.  241.) 

Imidocfo'phosphoric  acid, 
HO— PO  <I°1>  PO— OH. 

Correct   name   for   p?/rophosphaniic   acid. 
(Mente,  A.  248.  251.) 

Barium  imidodiphosphate,  Ba/O  >  po 
SI.  sol.  in  H2O.    (Mente,  A.  248.  243.) 


Barium  imidocfo'phosphate,  basic, 


/O.  po  / 

>  N—  Ba—  NX 


POH3s 


2H2O. 
Ppt.     (Mente.) 


396 


IMIDOPHOSPHATE,  FERRIC 


Ferric  imidocftphosphate. 

SI.  sol.  in  cone,  acids.    (Mente,  A.  248.  241.) 

Silver   imidod?  phosphate,   Ag3H2P2NO6. 

Insol.  in  H2O.     (Stokes,  Am.  Ch.  J.  1896, 
18.  660.) 

Ag4HP2NO6.    Ppt.      (Stokes.) 

Dumidodiphosphoric  acid, 
HO—  PO  <  Ng  >  po—  OH. 

Correct  name  for  p?/rophosphocfaamic  acid. 
(Mente,  A.  248.  241.) 

Barium    cfoimidocfophosphate, 


SI.   sol.   in   dil.   acids.     (Mente,   A.   248. 
244.) 

Sodium  (Mmidocftphosphate,  basic, 
/ONa 


\ONa. 
SI.  sol.  in  H2O.    (Mente,  A.  248.  245.) 

ZH'imidoJn'phosphoric  acid. 

Silver  dumido^nphosphate,  Ag3H4P3N2O8. 

Insol.  in  H2O.    Very  sol.  in  NH4OH-fAq. 

Rather  si.  sol.  in  dil.  HNO3.  (Stokes,  Am 
Ch.  J.  1896,  18.  657.) 

Ag5H2P3N2O8.  Insol.  in  H2O.  Very  sol.  in 
NH4OH+Aq. 

Decomp.  by  HNO3.    (Stokes.) 

Tnsodiumdumido^nphosphate, 

P3N208H4Na3. 
Sol.  in  H2O. 
Insol.  in  alcohol.     (Stokes.) 

Tn'imidotetfraphosphoric  acid. 

Silver  2nimidote£mphosphate. 

Ag4H5P4N3O]0. 
Ppt.     (Stokes,  Am.  Ch.  J.  1898,  20.  755.) 

Sodium  inimidofefraphosphate, 

P4N3010H5Na4. 

Easily  sol.  in  H2O;  insol.  in  sodium  acetate 
solution  and  dil.  alcohol.  (Stokes,  Am.  Ch. 
J.  1898,  20.  754.) 

Imidosulphamide,  NH2.SO2.NH.SO2.NH2. 

"Sulphamide"  of  Traube. 

Very  sol.  in  H2O  with  decomp.  appreci- 
ably sol.  in  cold,  easily  sol.  in  hot  methyl  and 
ethyl  alcohol.  Insol.  in  C6H6,  and  CHC13.  SI. 
sol.  in  ether,  cold  and  hot  acetic  ether  and 
glacial  acetic  acid.  Moderately  stable  toward 
alkalies.  (Hantzsch  and  Stuer,  B.  1905,  38. 
1022.) 


Ammonium  imidosulphamide, 

NH4S2O4N3H4. 
(Hantzch  and  Stuer.) 

Imidosulphonic  acid, 


Ammondisulphonic  acid  of  Glaus.  Known 
only  in  aqueous  solution.  (Divers  and  Haga, 
Chem.  Soc.  61.  943.) 

Very  unstable.    (Berglund,  B.  9.  252.) 

Ammonium  imidosulphonate,  basic, 

(NH4)N(S03NH4)2 

Sol.  in  9  pts.  of  H2O.    Solution  is  stable. 

Insol.  in  alcohol. 

SI.  sol.  in  warm  cone.  H2SO4  without  de- 
comp. (Rose,  Pogg.  1834,  32.  81.) 

Much  less  sol.  than  the  neutral  salt.  (Berg- 
lund, B.  9.  255.) 

=  "Parasulphatammon." 

+H2O.  Gradually  efflorescent.  Sol.  in 
H2O  with  subsequent  decomp.  (Divers  and 


Ammonium  imidosulphonate,  HN(SO3NH4)2. 
Sol.  in  H2O.    (Raschig,  A.  241. 161.) 

Ammonium  barium  imidosulphonate, 

NH4BaN(SO3)2(?). 

Very  si.  sol.  in  H2O.     (Divers  and  Haga.) 
(NH4)2Ba5N4(S08)8+8H2O.     (D.  and  H.) 

Ammonium  calcium  imidosulphonate. 
(Divers,  Chem.  Soc.  1892,  61.  968.) 

Ammonium   sodium  imidosulphonate, 

NH4Na5N2(SO3)4+7H2O,  and  2^H2O. 

Very  si.  sol.  in  NH4OH+Aq.    (Divers  and 
Haga.) 

Ammonium  sodium  imidosulphonate  nitrate, 

HN(S03NH4)2,  NaN03. 
Very  sol.  in  H2O.    (Divers  and  Haga.) 

Barium  imidosulphonate,  Ba[N(SO3)2Ba]2  + 

5H2O. 

SI.  sol.  in  H2O.    (Berglund,  B.  9.  255.) 
Sol.  in  dil.   HNO3+Aq  without  decomp. 

(Divers  and  Haga.) 
HN(SO3)2Ba+H2O.     Moderately   sol.   in 

H2O.    (D.  and  H.) 

Barium  mercury  imidosulphonate, 

N2Hg(S03)4Ba2. 

Almost  insol.  in  cold  H2O.     (Divers  and 
Haga,  Chem.  Soc.  1892,  61.  977.) 

Barium  sodium  imidosulphonate, 

Ba1iNa8N10(SO3)2o  +  13H2O. 
Sparingly  sol.   in  H2O.     Readily  sol.   in 
HNO3  or  HC1.     (Divers,  Chem.  Soc.  1892, 
61.  967.) 


IMIDOSULPHOPHOSPHATE,  AMMONIUM  HYDROGEN 


397 


Calcium  imidosulphonate,  Ca[N(SO3)2Ca]2  + 

6H20. 
SI.  sol.  in  H2O.    (Berglund.) 

Calcium  mercury  imidosulphonate, 

N2Hg[(S03)2Ca]2. 

Very  sol.  in  H2O.     (Divers  and  Haga, 
Chem.  Soc.  1896,  69.  1629.) 

Calcium  mercury  imidosulphonate  chloride, 

(NS,0«Ca),Hg,Cl+12H,0. 
Decomp.   by   H2O.      (Divers   and   Haga, 
Chem.  Soc.  1896,  69.  1629.) 

Calcium  sodium  imidosulphonate, 

NaN(SO3)2Ca+3H2O. 
SI.  sol.  in  cold  H20.     (Divers  and  Haga, 
Chem.  Soc.  61.  968.) 

Lead  imidosulphonate,  (PbOHSO3)2NPbOH. 
Ppt.    (Berglund.) 

Insol.  in  H2O.    (Divers  and  Haga.) 
(PbOH)3N(SO3)2,   PbO.     Insol.   in   H2O; 

easily  sol.  in  dil.  HNO3+Aq.    (D.  and  H.) 

Mercurous  imidosulphonate,  basic, 

[Hg2N(S03)2Hg2]2O+6H2O. 
Much  more  sol.  in  dil.  HNO3  than  mer- 
curic   salt.      Sol.    in    cold    cone.      KI+Aq, 
leaving  half  Hg  as  metal.    (Divers  and  Haga, 
Chem.  Soc.  1896,  69.  1631.) 

Mercuric  imidosulphonate,  basic, 

NH(S03,  HgO)2Hg. 
Easily  decomp.    (Divers  and  Haga.) 

Mercuromercuric  imidosulphonate, 
[HgnN(SOa)«HgI],0+3H,0. 

(Divers  and  Haga.) 

[HgnN(S03)2Hg'2]20,    [Hg'2N(S03)2Hg2, 
HgnN(SO3)2HgI2]O+6H2O.        (Divers      and 
Haga.) 

Mercury  sodium  imidosulphonate,  basic, 

Hg2ON(SO3)2Na+2H2O. 
Slightly  efflorescent.  Decomp.  by  long 
washing  with  H2O.  Much  more  readily  sol. 
in  HC1  than 'in  HNO3  or  H2SO4  and  is  wholly 
decomp.  thereby.  (Divers  and  Haga,  Chem. 
Soc.  1892,  61.  983.) 

Mercury  sodium  imidosulphonate, 
HgN2(SO3Na)4+6H2O. 

Sparingly  sol.  in  cold  H2O. 

Readily  sol  in  HNO3  and  in  HC1. 

Decomp.  by  HC1  immediately,  but  not 
by  HN03.  (Divers  and  Haga,  Chem.  Soc. 
1892,  61.  981.) 

Potassium  imidosulphonate,  basic, 

KN(S03K)2+H20. 
Sol.  in  H2O.    (Raschig,  A.  241.  161.) 
Less  sol.  than  neutral  salt.    (Berglund.) 


Potassium  imidosulphonate,   HN(SO3K)2. 

Sol.  in  H2O.    (Raschig,  A.  241.  161.) 

=  Potassium  ammoncfosulphonate  of  Glaus. 

Difficultly  sol.  in  cold  H2O,  sol.  in  64  pts. 
H2O  at  23°.  (Fremy.)  Gradually  decomp. 
by  boiling.  (Glaus.) 

SI.  sol.  in  H2O.    (Berglund,  B.  9.  255.) 

Potassium  mercury  imidosulphonate, 

N2Hg(SO3K)4+4H2O. 
See  Mercurimidosulphonic  acid. 

Silver   imidosulphonate,    AgN(SO3Ag)2. 
SI.  sol.  in  H2O.    (Berglund.) 

Silver  sodium  imidosulphonate, 

NaN(S03Ag)2. 

SI.  sol.  in  H2O.    (Divers  and  Haga.) 
AgNa2N(S03)2.    SI.  sol.  in  H2O,  but  more 
sol.  than  the  two  preceding  salts.    (D.  and  H.) 

Sodium  imidosulphonate,  HN(SO3Na)2  + 

2H2O. 

Not  efflorescent.  Very  sol.  in  H2O.  (Diver 
and  Haga.) 

NaN(SO3Na)2+12H2O,  Efflorescent.  SI. 
sol.  in  cold  H2O,  but  very  sol.  in  hot  H2O. 
Sol.  in  5.4  pts.  H20  at  27.5°.  (Divers  and 
Haga.) 

Sodium  strontium  imidosulphonate, 

SrNaNS2O6+3H2O. 

SI.  sol.  in  H2O.  (Divers,  Chem.  Soc. 
1896,  69.  1625.) 

Strontium  imidosulphonate, 

Sr[N(S03)2Sr]2+6H20. 
SI.  sol.  in  H2O.    (Berglund.) 
+12H2O.      Somewhat    sol.    in   hot    H2O. 
(Divers,  Chem.  Soc.  1896,  69.  1623.) 

Imido2nsulpho0r£/w>phosphoric  acid, 

NH:P(SH)3. 

Insol.  in  CS2  and  readily  decomp.  by  H2O. 
(Stock,  B.  1906,  39.  1991.) 

Ammonium  imido/nsulphoo?  ^ophosphate, 
NHP(SNH4)3. 

Very  hydroscopic. 

Loses  NH3  in  the  air. 

Somewhat  sol.  in  liquid  NH3. 

Decomp.  by  any  other  solvent  in  which 
it  is  sol.  (Stock,  B.  1906,  39. 1983.) 

Diammonium  hydrogen  imido^nsulphoor^o- 

phosphate,  SHP(SNH4)2NH. 
(Stock,  B.  1906,  39.  1983.) 


Ammonium  ^'hydrogen 
SNH4P(SH)2NH. 

(Stock.) 


398 


IMIDOSULPHOPHOSPHATE,  SODIUM  HYDROGEN 


Di sodium  hydrogen  imido^nsulphcor^ophos- 

phate,  SHP(SNa)2NH. 
Very  easily  sol.  in  H2O.    Decomp.  by  H2O. 
Somewhat  sol.  in  methyl  and  ethyl  alcohol. 
(Stock.) 

Z)iimidopentasulphop2/rophosphoric  acid, 

P2S5N2H6. 

Not  known  in  pure  state.  (Stock,  B. 
1906,  39.  1967.) 

Ammonium  diimidopentasvlphopyrophos- 
phate,  S[P(SNH4)2NH]2. 

Very  hydroscopic. 

Sol.  in  cold  H2O  with  decomp.  (Stock,  B. 
1906,  39.  1978.) 

Inidosulphurous  acid. 

Ammonium  imidosulphite,  HN(SO2NH4)2. 

Somewhat  deliquescent. 

Very  unstable.  Easily  sol.  in  H2O  with 
decomp;  into  thiosulphate  and  amidosul- 
phate. 

Insol.  in  alcohol.  (Divers  and  Ogawa, 
Chem.  Soc.  1901,  79.  1100.) 

Ammonium  barium  imidosulphite, 

Ba(SO2NHSO2NH4)2. 
Sol.  in  H2O.     (Divers,  Chem.  Soc.  1901, 
79.  1102.) 

Potassium  imidosulphite,  NH(S02K)2. 
(Divers   and   Owaga,    Proc.    Chem.    Soc. 

1900,  16.  113.) 

Very  sol.  in  H20.     (Divers,  Chem.  Soc. 

1901,  79.  1101.) 

Imidosulphuryl  amide,  S2O4N3H5  = 


S02< 
S02< 


NH2 

NH 

NH2. 


Sol.  in  NH4OH-f-Aq.     Decomp.  by  cone. 
HC1.     Insol.  in  alcohol  sat.  with  NH3. 
(Mente,  A.  248.  265.) 

Indie  acid. 

Magnesium  indate,  MgIn2O4+3H2O. 

Ppt.  Insol.  in  H2O.  Sol.  in  HCl+Aq. 
(Renz,  B.  1901,  34.  2764.) 

Indium,  In. 

Does  not  decomp.  hot  H2O. 

Sol.  in  dil.  HC1,  and  H2SO4+Aq.  Decomp. 
by  cone.  H2SO4.  Easily  sol.  in  HNO3+Aq. 
Insol.  in  acetic  acid.  Insol.  in  KOH-j-Aq. 
(Winkler,  J.  pr.  102.  273.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  830.) 

Yz  com.  oleic  acid  dissolves  0.0039  g.  In  in 
6  days.  (Gates,  J.  phys.  Chem.  1911,  15. 
143.) 


Indium  monobromide,  InBr. 

Decomp.  by  hot  H2O.  Easily  sol.  in  acids. 
Easily  sol.  in  cold  cone.  HC1.  (Thiel,  Z. 
anorg.  1904,  40.  328.) 

Indium  ^bromide,  InBr2. 

Decomp.  by  hot  H2O.  Easily  sol.  in  acids. 
(Thiel,  Z.  anorg.  1904,  40.  329.) 

Indium  fhbromide,  InBr3. 

Deliquescent.    Very  sol.  in  H2O. 

Indium  monochlciide,  InCl. 

Deliquescent.  Decomp.  by  H2O  into  InCl3. 
and  In.  (Nilson  and  Pettersson,  Chem.  Soc. 
43.  820.) 

Indium  ^chloride,  InCl2. 

Deliquescent  in  moist  air;  decomp.  by  F2O 
into  InCl3  and  In.  (Nilson  and  Pettersson, 
Chem.  Soc.  43.  818.) 

Indium  frzchloride,  InCl3. 

Very  deliquescent;  sol.  in  H2O  with  hissing 
and  great  evolution  of  heat. 

Indium  lithium  chloride. 

Extremely  deliquescent.  Sol.  in  H2O. 
(Meyer,  A.  150.  144.) 

Indium  potassium  chloride,  3KC1,   InCl3  + 

1^H20. 
Easily  sol.  in  H2O.    (Meyer.) 

Indium  Znfluoride,  InF3+3H2O. 

Sol.  in  H2O;  readily  decomp.  (Thiel,  B. 
1904,  37.  175.) 

1  1.  H2O  dissolves  86.4  g.  at  25°.  Decomp. 
on  boiling.  (Thiel,  Z.  anorg.  1904,  40.  331.) 

+9H2O.    SI.  sol.  in  cold  H2O. 

Sol.  in  HC1  and  in  HNO3. 

Insol.  in  alcohol  and  ether.  (Chabrie, 
C.  R.  1905,  140.  90.) 

Indium  hydrosulphide. 

Decomp.  by  acids.    (Meyer.) 

Indium  hydroxide,  In2O6He. 

Sol.  in  acids;  also  in  KOH,  or  NaOH+Aq 
but  the  solution  clouds  up  on  standing  or 
boiling,  with  separation  of  In2O6H6.  Insol.  in 
NH4OH,  or  NH4Cl+Aq. 

SI.  sol.  in  NH4OH+Aq.  (Renz,  B.  1904,  37. 
2110.) 

SI.  sol.  in  alkylamines  but  completely  ppt. 
by  addition  of  the  hydrochloride  of  the  base. 
(Renz,  B.  1903,  36.  2754.) 

Indium  rrconoiodide,  Inl. 

Slowly  decomp.  in  moist  air.  Not  attacked 
by  boiling  H2O. 

Sol.  in  dil.  HNO3  in  presence  of  AgNO3. 
Very  slowly  sol.  in  cold,  more  rapidly  sol.  in 


IODAURICYANIDE,  BARIUM 


399 


hot  acids  with  evolution  of  H2.    Very  sol.  in 
sulphurous  acid. 

Insol.   in   alcohol,   ether  and   chloroform. 
(Thiel,  Z.  anorg.  1910,  66.  302.) 

Indium  ohiodide,  InI2. 

(Thiel,  Z.  anorg.  1910,  66.  302.) 

Indium  tfniodide,  InI3. 

Deliquescent.    (Meyer.) 

Sol.inCHCls.    Decomp.  byxylene.    (Thiel, 
Z.  anorg.  1904,  40.  330.) 

Indium  nitride,  InN. 

Decomp.    by    heat.      (Franz    Fischer,'  B. 
1910,  43.  1469.) 

Indium  monoxide,  InO. 

Gradually  sol.  in  HCl+Aq.     (Winkler,  J. 
pr.  94.  1.) 


Indium  sesquioxide, 

Slowly  sol.  in  cold,  easily  in  hot  acids. 
Four  modifications: 

(1)  Yellow.     Amorphous.     Sol.  in  acids. 
Its  hydroxide  is  insol.  in  ammonia  and  NH4C1. 

(2)  White.     Amorphous.     Insol.  in  acids. 

(3)  White.      Amorphous.      Sol.    in    acids. 
Its  hydroxide  is  sol.  in  ammonia,  but  pptd.  by 
NH4C1. 

(4)  Crystallized.     Crystalline  modification 
is  insol.  in  acids.     (Renz,  B.  1904,  37.  2112.) 

Insol.  in  liquid  NH3.     (Gore,  Am.  Ch.  J. 
1898,  20.  830.) 

Indium  oxide,  In7O9  =  3InO,  2In203  (?). 
(Winkler.) 
In4O5  =  2InO,  In2O3  (?).     (Winkler.) 

Indium  oxy  bromide  (?). 

Not  decomp.  by  hot  acids  or  alkalies. 
(Meyer,  A.  150.  137.) 

Indium  oxychloride,  InOCl. 

Very  si.  sol.  in  H2O.    (Thiel,  B.  1904,  37. 
176.) 

Very  si.  sol.  in  cold  or  hot  dil.   acids. 
Quickly  sol.  in  hot  cone,  acids.     (Thiel,  Z. 
anorg.  1904,  40.  327.) 

Indium  Znselenide,  In2Se3. 

Sol.  in  strong  acids  with  evolution  of  H2Se. 
(Thiel,  Z.  anorg.  1910,  66.  315.) 

Diindium  sulphide,  In2S. 

Sol.  in  acids.    (Thiel,  Z.  anorg.  1904,  40. 
326.) 

Indium  monosulphide,  InS. 

Easily  sol.  in  HC1  with  evolution  of  H2S. 

Sol.  in  HNO3  with  evolution  of  oxides  of 
nitrogen.     (Thiel,  Z.  anorg.  1910,  66.  314.) 


Indium  sesgiasulphide,  In2S3. 
Partially  sol.  in  (NH4)2S+Aq. 

Indium  potassium  sulphide,  In2S3,  K2S. 

Insol.  in  H2O;  decomp.  by  weak  acids  with 
separation  of  In2S3;  sol.  in  cone,  acids. 
(Schneider,  J.  pr.  (2)  9.  209.) 

Indium  silver  sulphide,  In2S3,  Ag2S. 
Insol.  in  H2O.    (Schneider,  I.  c.) 

Indium  sodium  sulphide,  In2S3,  Na2S-f-2H20. 
Insol.  in  H2O.    (Schneider,  I.  c.) 

Indium  wonotelluride,  InTe. 

Sol.  in  HNO3;  insol.  in  HCl+Aq.  (Thiel, 
Z.  anorg.  1910,  66.  318.) 

Infusible  white  precipitate. 

ZXiodamine,  NHI2. 
Decomp.  by  H2O. 

lodammonium  iodide,  NIH3I. 

Decomp.  by  H2O,  caustic  alkalies,  and 
acids.  Sol.  in  KI+Aq,  alcohol,  ether.  CS2, 
CHC13.  (Guthrie,  Chem.  Soc.  (2)  1.  239.) 

lodauric  acid,  HAuI4  (?). 
Not  known  with  certainty. 

Ammonium  iodaurate. 

Deliquescent.  Decomp.  by  H2O.  (John- 
ston, Phil.  Mag.  (3)  9.  266.) 

Barium  iodaurate. 
Sol.  in  BaI2+Aq. 

Caesium  iodaurate,  CsAuI4. 

(Gupta,  J.Am.  Chem.  Soc.  1914,  36.  748.) 

Ferrous  iodaurate. 

Sol.  inH2O.    (Johnston.) 

Potassium  iodaurate,  KAuI4. 

Decomp.  by  H2O.    Sol.  in  KI,  and  HI-fA. 

(Johnston.) 

Sodium  iodaurate. 

Very  deliquescent.    (Johnston.) 

lodauricyanhydric  acid,  HAu(CN)2I2. 
Known  only  in  its  salts. 

Barium    iodauricyanide,     Ba[Au(CN)2I2]2  + 

10H2O. 

SI.  sol.  in  cold,  easily  in  hot  H2O.  Easily 
sol.  in  alcohol.  (Lindbom,  Lund.  Univ.  Arsk. 
12.  No.  6.) 


400 


IODAURICYANIDE,  CALCIUM 


Calcium    iodauricyanide,    Ca[Au(CN)2I2]2  + 

10H2O. 
Not  stable.     (L.) 

Cobalt  iodauricyanide,  Co[Au(CN)2I2]2  + 

10H2O. 

Most  insol.  of  all  iodauricyanid.es,  and  only 
si.  sol.  in  warm  H2O.  Easily  sol.  in  alcohol. 

Potassium    iodauricyanide,     KAu(CN)2I2  + 

H2O. 

SI.  sol.  in  cold,  easily  sol.  in  warm  H2O  and 
alcohol.  (L.) 

Strontium  iodauricyanide,  Sr[Au(CN)2I2]2  + 

10H2O. 
SI.  sol.  in  cold,  more  easily  in  hot  H2O. 

lodhydric  Acid,  HI. 

Very  easily  and  quickly  absorbed  by  H2O, 
with  evolution  of  much  heat. 

Solution  is  decomp.  on  exposure  to  the  air. 

1  vol.  H20  absorbs  450  vols.  HI  at  10°. 
(Thomson.) 

I  vol.  H2O  absorbs  425  vols.  HI  at  10°. 
(Berthelot,  C.  R.  76.  679.) 

Weak  or  strong  solutions  when  boiled  in  an 
atmosphere  of  H  leave  a  residue  of  constant 
composition,  which  distils  unchanged  at  126° 
(de  Luynes),  at  127°  (Roscoe,  Chem.  Soc.  13. 
146;  Naumann;  Topsoe),  at  128°  (Bineau,  A. 
ch.  (3)  7.  266);  and  has  a  sp.  gr.  of  1.67  (Nau- 
mann), of  1.70  (Bineau,  de  Luynes),  of  1.708 
(Topsoe);  and  contains  56.26  %  HI  (Bineau), 
57.0%  HI  (Roscoe),  57.75%  HI  (Topsoe.) 

By  conducting  dry  H  gas  through  the 
aqueous  solution  of  HI,  a  constant  residue  is 


Solution  in  H2O  sat.  at  0°  has  sp.  gr.  =  1 . 99 
(de  Luynes,  A.  ch.  (4)  2.  385);  2.0  (Vigier). 

Sp.gr.  of  HI +Aq. 


Sp.  gr. 

%  HI 

Temp. 

1.017 

2.286 

13.5° 

1.0524 

7.019 

13.5 

1.077 

10.15 

13.5 

1.095- 

12.21 

13 

1.102 

13.09 

13.5 

.126 

15.73 

13.5 

.164 

19.97 

13.5 

.  .191 

22.63 

13.8 

.225 

25.86 

13.8 

.2535 

28.41 

13.5 

1.274 

30.20 

13.5 

1.309 

33.07 

13 

1.347 

36.07 

13 

1.382 

38.68 

13 

1.413 

40.45 

13 

1.451 

43.39 

13 

1.4865 

45.71 

13 

1.528 

48.22 

13 

1.542 

49.13 

13.5 

.5727- 

50.75 

13 

.603 

52.43 

12.5 

.630 

53.93 

14 

.674 

56.15 

13.7 

.696 

57.28 

13 

.703 

57.42 

12.5 

.706 

57.64 

13.7 

.708 

57.74 

12 

(Topsoe,  B.  3.  403.) 


Sp.  gr.  of  HI+Aqat  15°. 


ODcamea,  containing  ou.o-uu./  ~/0  JO.JL  11  temp, 
is  15-19°,  and  58.2-58.5%  HI  if  temp,   is 

%HI 

Sp.  gr. 

%HI 

Sp.  gr. 

%HI 

Sp.  gr. 

100°.    (Roscoe.) 

1 

1.008 

21 

1.175 

41 

1.414 

Solubility  of  HI,  in  H2O  at  t°. 

2 
3 

1.015 
1.022 

22 
23 

1.185 
1.195 

42 
43 

1.429 
1.444 

t° 

%  HI 

Solid  Phase 

4 

1.029 

24. 

1.205 

44 

1.459 

5 

1.037 

25 

1.216 

45 

.475 

-10 

20.3 

Ice 

6 

1.045 

26 

1.227 

46 

.491 

-20 

29  3 

7 

1.053 

27 

1.238 

47 

.508 

—  30 

35  1 

8 

1.061 

28 

1.249 

48 

.525 

-40 

39 

9 

1.069 

29 

1.260 

49 

.543 

—  50 

42 

10 

1.077 

30 

1.271 

50 

.561 

-60 

44.4 

11 

1.085 

31 

1.283 

51 

.579 

-70 

46.2 

12 

1.093 

32 

1.295 

52 

.597 

-80 
-60 

47.9 
52.6 

Ice+HI,  4H2O 
HI,  4H2O 

13 

14 

1.102 
1.110 

33 
34 

1.307 
1.320 

53 
54 

.615 
.634 

-40 

59 

15 

1.118 

35 

1.333 

55 

.654 

—  35.5 

64 

16 

1.127 

36 

1.346 

56 

.674 

-40 

65  5 

17 

1.137 

a7 

1.359 

57 

.694 

-49 

—  48 

66.3 
70.3 

HI,4H2O+HI,  3H2O 
HI,  3H2O 

18 
19 

1.146 
1.155 

38 
39 

1.372 
1.386 

58 

.713 

-56 

73.5 

HI,3H2O+HI,2H2O 

20 

1.165 

40 

1.400 

-52 

74 

HI,  2H2O 

(Topsoe,  calculated  by  Gerlach,  Z.  anal.  27. 

(Pickering,  B.  1893,  26.  2307.) 

316.) 

IODATE,  AMMONIUM 


401 


Sp.  gr.  of  HI+Aqatl5°. 

Sp.  gr.  of  HIO3-f  Aq  at  15°. 

%HI 

Sp.  gr. 

%HI 

Sp.  gr. 

%HI 

Sp.  gr. 

%I^ 

Sp.  gr. 

%  I205 

Sp.  gr. 

5 

1.045 

25 

1.239 

45 

1.533 

1 

1.0053 

35 

.4428 

10 
15 

1.091 
1.138 

30 
35 

1.296 
1.361 

50 
52 

1.650 
1.700 

5 
10 

1.0263 
1.0525 

40 
45 

.5371 
.6315 

20 

1.187 

40 

1.438 

15 

20 

1.1223 
1.2093 

50 
55 

.7356 
.8689 

25 

1.2773 

60 

.9954 

Only  a  "  moderate  degree  of  accuracy  "  is 

30 

1.3484 

6$ 

2.1269 

claimed  for  this  table. 
253.) 

Mpt.— 43° 


+2H2O. 
26.  2308.) 
+3H2O. 
+4H2O. 


(Pickering,  B.  1893, 


Mpt.— 48°.    (Pickering.) 
Mpt.— 36.5°.     (Pickering.) 


lodic  acid,  HIO3. 

Very  sol.  in  H2O  and  alcohol. 

100  g.  H2O  dissolve  286.1  g.  HIO3  at  13.5°. 
Sp.  gr.  of  HIO3+Aq.  =2.4256. 

100  g.  H2O  dissolve  293  g.  HIO3  at  18°. 
Sp.  gr.  of  HIOa+Aq.  =2.4711. 

(Groschuff,    Z.   anorg.    1905,    47.   337.) 

Solubility  of  HIO3  in  H2O  at  t°. 


Solid  phase 

t° 

G.  HI03  in 
100  g.  of  the 
solution 

G.  I2O5  in 
100  g.  of  the 
solution 

ice 

—  0.30 

1.78 

1.69 

u 

—  0.67 

4.35 

4.13 

tt 

—  1.01 

7.17 

6.81 

u 

—  1.90 

17.66 

16.75 

u 

—  2.38 

27.65 

26.22 

« 

—  4.72 

54.19 

51.42 

u 

—  6.32 

60.72 

57.61 

(( 

—12.25 

71.04 

67.40 

(I 

—13.5 

72.2 

68.5 

u 

—15 

73.8 

70.0 

'    it 

—19 

76.2 

72.3 

ice+HIO3 

—14 

72.8 

69.1 

HIO3 

0 

74.1 

70.3 

11 

+  16 

75.6 

71.7 

<( 

40 

77.7 

73.7 

u 

60 

80.0 

75.9 

u 

80 

82.5 

78.3 

H 

85 

83.0 

78.7 

U 

101 

85.2 

80.8 

HI03+HI308 

110 

86.5 

82.1 

HI308 

125 

87.2 

82.7 

u 

140 

88.3 

83.8 

u 

160 

90.5 

85.9 

(Groschuff,  Z.  anorg.  1905,  47.  343.) 

Sat.  solution  has  sp.  gr.  2.842  at  12.5°,  and 
boils  at  104.°  (Ditte,  B.  6.  1533.)  Sat.  solu- 
tion has  sp.  gr.  2.1629  (1.874  pts.  I2O5  in  1  pt. 
H2O)  at  13°,  and  boils  at  100°.  (Kammerer, 
Pogg.  138.  400.) 


(Kammerer.) 

According  to  Thomsen  (B.  7.  71)  solutions 
of  HIO3  have  sp.  gr.  — 

HIO3+  10H2O  =  1.6609. 
HIO3+  20H2O  =  1.3660. 
HIO3+  40H2O  =  1.1945. 
HIO3+  80H2O  =  1.1004. 
HIO3  +  160H2O  =  1.0512. 
HIO3+320H2O  =  1.0258. 

H2SO4  at  nearly  boiling  temp,  dissolves  Vi 
its  weight  of  iodic  acid.  (Millon.) 

Solubility  in  HNO3  containing  27.73%  HNO3. 
100  g.  of  the  sat.  solution  contain  at: 
0°        20°        40°        60° 
18        21         27         38  g.  HIO3. 

Solubility  in  HNO3  containing  40.88%  HNO3. 

100  g.  of  the  sat.  solution  contain  at: 

0°       20°        40°        60° 

9         10          14          18  g.  HIO3. 

(Groschuff,   Z.   anorg.    1905,   47.   344.) 

Less  sol.  in  HNO3  than  H2O;  nearly  insol. 
in  anhydrous  HNO3.  (Groschuff,  Z.  anorg. 
1905,  47.  347.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  830.)  • 

Unattacked  and  undissolved  by  liquid  NOj. 
(Frankland,  Chem.  Soc.  1901,  79.  1362.) 

Insol.  in  absolute  alcohol.  Alcohol  of  35° 
B.  dissolves  half  its  weight  in  HIO3.  (Kam- 
merer.) 


(Grosschuff,  Z.  anorg.  1905, 


HIO3,  I2O6. 

47.  343.)  • 


lodates. 

The  alkali  iodates  are  sol.  in  H2O,  the  others 
are  si.  sol.  or  insol.  therein. 

Aluminum  iodate,  A1(IO3)3  (?). 
Deliquescent.    (Berzelius.) 

Ammonium  iodate,  NH4IO3. 

SI.  sol.  in  H2O.    Sol.  in  38.5  pts.  H2O  at  15°, 
6.9  pts  .at  100°.     (Rammelsberg,  Pogg.  44. 

555.) 


402 


IODATE,  AMMONIUM 


Solubility  of  NH4IO3  in  HIO8+Aq  at  30°. 


%  HI03 

%  NHJOa 

in  the 

in  the 

Solid  phase 

solution 

solution 

0 

4.20 

NH4IO3 

2.54 

3.89 

* 

4.52 

3.83    . 

NH4IO3+NH4IO3,  2HIO3 

4.51 

3.86 

4.56 

3.75 

4.73 

3.53- 

NHJO    2H103 

6.57 

1.94 

8.45 

1.09 

9.12 

0.89 

24.00 

0.62 

36.01 

0.41 

44.43 

0.39 

58.12 

0.37 

76.35 

0.31 

NHJ03,  2HI03+HI03 

76.70 

0 

HI03 

(Meerburg,  Z.  anorg.  1905,  45.  341.) 

,  +H2O.     (Ditte,  A.  ch.  (6)  21.  146.) 

Ammonium  cfoiodate,  NH4H(IO3)2. 

SI.  sol.  in  cold  H2O.  (Ditte,  A.  ch.  (6)  21. 
145.) 

Ammonium  /niodate,  NH4H2(IO3)3. 

Sol.  in  H2O.  (Blomstrand,  J.  pr.  (2)  42. 
335.) 

See  also  solubility  in  H1O3,  under  Am- 
monium iodate.  (Meerburg.) 

Ammonium  cobalt  iodate. 

Decomp.  by  H2O.  Insol.  in  alcohol. 
(Rammelsberg.) 

Ammonium     manganic     iodate,     Mn(IO3)4, 

2NH4I03. 

Ppt.  Insol.  in  H2O.  Insol.  in  HIO3.  (Berg, 
"C.  R.  1899,  128.  675.) 

Ammonium  oxydimercuriammonium  iodate. 
See    Oxyd^mercuriammonium    ammonium 
iodate. 

Ammonium  tellurium  iodate. 
See  lodotellurate,  ammonium. 

Ammonium  iodate  selenate. 
See  lodoselenate,  ammonium. 

Barium  iodate,  Ba(IO3)2. 

Anhydrous  salt  is  sol.  in  1746  pts.  H2O  at 
15°,  and  600  pts.  H2O  at  100°  (Rammelsberg, 
Pogg.  44.  577);  in  3018  pts.  H2O  at  13.5°,  and 
681  pts.  H2O  at  100°.  (Kremers,  Pogg.  84. 
27.) 


Solubility  of  Ba(IO,)2  in  H2p,  100  g.  sat. 
Ba(IO3)2+Aq  at  t°  contain  g.  anhydrous 
Ba(I03)2. 


03  ^. 

to  f' 

03    " 

t° 

is 

t° 

1 

t° 

§2 

O  08 

O  c3 

O  c3 

« 

w 

n 

Eutectic  point 

—0.046°  ±0.002° 

0.008 

30° 

0.031 

70° 

0.093 

+  10° 

0.014 

40° 

0.041 

80° 

0.115 

20° 

0.022 

50° 

0.056 

90° 

0.141 

25° 

0.028 

60° 

0.074 

*99  .  2° 

0.197 

*Bpt.  at  735  mm.  pressure  =  about  100°  at 
760  mm.  pressure. 

(Anschiitz,  Z.  phys.  Ch.  1906,  56.  241.) 

1  1.  sat.  aq.  solution  contains  0.284  g. 
Ba(IO3)2  at  room  temp.  (Hill  and  Zink,  J. 
Am.  Chem.  Soc.  1909,  31.  44.) 

1  1.  H2O  dissolves  0.3845  g.  Ba(IO3)2  at 
25°.  (Harkins  and  Winninghof,  J.  Am. 
Chem.  Soc.  1911,  33.  1828.) 

Easily  sol.  in  cold  HCl+Aq;  difficultly  sol. 
in  warm  HNO3+Aq.  (Rammelsberg.) 

Insol.  in  H2SO4.    (Ditte.) 

100  cc.  NH4OH+Aq  (sp.  gr.=0.90)  dis- 
solve 0.0199  g.  Ba(IO3)2.  (Hill  and  Zink.) 

Solubility  in  salts +Aq  at  25°. 

C  =  concentration  of  salt  in  salt  solution 
expressed  in  equivalents  per  1. 

S=solubility  of  Ba(IO3)2  in  salts+Aq  ex- 
pressed in  equivalents  per  1. 


Salt 

c 

s 

Ba(N03)2 

0.001 
0.002 
0.005    . 
0.020 
0.050 
0.100 
0.200 

0.001362 
0.001212 
0.0009753 
0.0006744 
0.0006131 
0.0005659 
0.0005580 

KNO3 

0.002 
0.010 
0.050 
0.200 

0.001624 
0.001820 
0.002640 
0.003190 

KIO3 

0.00010608 
0.0005304 
0.0010608 

0.001510 
0.001242 
0.0009418 

(Harkins  and  Winninghof,  J.  Am.  Chem.  Soc. 
1911,  33.  1829.) 

Insol.  in  alcohol. 

100  cc.  95%  alcohol  dissolve  0.0011  g. 
Ba(IO3)2  at  room  temp.  (Hill  and  Zink.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014.) 

+H2O.  Sol.  in  3333  pts.  H2O  at  18°,  and 
625  pts.  H2O  at  100°.  (Gay-Lussac,  A.  ch. 
91.  5.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329.) 


IODATE,  COBALTOUS 


403 


Barium  manganic  iodate, 
Mn(IO3)4,  Ba(IO3)2. 

Insol.  in  H2O. 

Insol.  in  HIO3.     (Berg,  C.  R.  1899, 
675.) 


128. 


Bismuth  iodate,  basic. 

Insol.  in  H2O.  Very  difficultly  sol.  in 
HNO3+Aq.  (Rammelsberg,  Pogg.  44.  568.) 
;  Bi(IO3)3+l^H2O.  Insol.  in  H2O. 

Cadmium  iodate,  Cd(IO3)2. 

Very  si.  sol.  in  H2O.  Easily  sol.  in  HNO3, 
or  NH4OH+Aq.  Sol.  in  Cd(C2H3O2)2  + 
Aq.  (Rammelsberg,  Pogg.  44.  566.) 

+H2O.  SI.  sol.  in  H2O.  Very  sol.  in  dil. 
HNOg+Aq.  (Ditte,  A.  ch.-  (6)  21.  145.) 

Cadmium  iodate  ammonia,  Cd(IO3)2,  2NH3. 

Insol.inH2O;sol.inNH4OH+Aq.  (Ditte.) 
A.  ch.  (6)  21.  145.) 

Cd(IO3)2,2NH3+H2O.   As  above.    (Ditte. 

Caesium  iodate,  CsIO3. 

100  pts.  H2O  dissolve  2.6  pts.  CsIO3  at  24°. 
Insol.  in  alcohol.  (Wheeler,  Sill.  Am.  J.  144. 
123.) 

2CsIO3, 12O5.  100  pts.  H2O  dissolve  2.5  pts. 
at  21°.  Not  decomp.  by  hot  H2O.  (Wheeler.) 

2CsIO3,  I2O5,  2HIO3.  SI.  sol.  in  cold  H20. 
and  decomp.  thereby  into  2CsIO3,  I2Os. 
(Wheeler.) 

Caesium  iodate  chloride,  CsCl,  HIO3. 

Decomp.    by    H2O    into    2CsIO3,     I2O5. 

(Wheeler.) 

Caesium  hydrogen  iodate  periodate, 

HCsIO3,  IO4+2H2O. 

,  Ppt.    Sol.  in  dil.  HNO3.    (Wells,  Am.  Ch. 
J.  1901,  26.  280.) 

Calcium  iodate,  Ca(IO3)2. 

100  pts.  dissolve  0.22  pt.  at  18°,  and 
0.986  pt.  at  100°.  (Gay-Lussac.)  Sol,  in 
cone.  HCl+Aq.  (Filhol.)  Much  more  sol. 
in  HNO3+Aq  than  in  H2O.  (Rammelsberg.) 
Insol.  in  H2SO4.  (Ditte.)  Scarcely  sol.  in 
sat.  KIO3+Aq.  (Sonstadt,  C.  N.  29.  209.) 

+H2O.       Sat.     solution     contains     at: 


21° 
0.37 

35° 
0.48 

40° 
0.52 

45° 
0.54%Ca(I03)2, 

50° 
0.59 

60° 
0.65 

80° 
0.79 

100° 

0.94%Ca(I03)2. 

(Mylius  and  Funk,  B.  1897,  30.  1724.) 

-f6H2O.    Efflorescent. 
Sol.  in  253  pts.  H2O  at  15°,  and  75  pts.  at 
100°.    (Rammelsberg.) 


Sat.  solution  contains  at: 

0°  10°  18°          30° 

0.1        0.17        0.25        0.42%  Ca(IO3)2, 
40°         50°          54°  60° 

0.61       0.89       0.14         1.36%Ca(IO3)2. 

(Mylius  and  Funk,  B.  1897,  30.  1724.) 

Much  more  sol.  in  HNO3+Aq.  Pptd.  by 
alcohol  from  Ca(IO3)2+Aq. 

Insol.  in  H2SO4.     (Ditte.) 

Pptd.  by  alcohol  from  aqueous  solution. 
(Henry.) 

Cerous  iodate,  Ce(IO3)3+2H2O. 

SI.  sol.  in  cold,  easily  sol.  in  hot  H2O  and  in 
acids.  (Holzmann,  J.  pr.  76.  321.) 

Solubility  in  H2O.  100  cc.  of  the  sat. 
solution  contain  0.1456  g.  at  25°.  (Rimbach, 
Z.  phys.  Ch.  1909,  67.  199;) 

Calc.  from  electrical  conductivity  of 
Ce(IO3)3+Aq.,  100  cc.  of  the  sat.  solution 
contain  0.1636  g.  Ce(I03)3  at  25°.  (Rim- 
bach,  Z.  phys.  Ch.  1909,  67.  199.) 

Ceric  iodate,  Ce(IO3)4. 

Slightly  hydrolyzed  by  H2O. 

0.34  g.  is  sol.  in'  100  cc.  hot  cone.  HNO3. 
(Barbieri,  Chem.  Soc.  1907,  92.  (2)  467.) 

Cobaltous  iodate,  Co(IO3)2. 

Anhydrous.  Sol.  in  warm  dil.  H3PO4,  or 
H2SO4+Aq.  (Ditte,  A.  ch, (6)  21.  14.) 

Solubility  in  H2O 


Form 

Temp. 

CO(I03)2 

Mots,  of 
water  free 
salt  to  100 
mols  H2O 

Co(I03)2+4H20 

0° 

0.54 

0.028 

tt 

18° 

0.83 

0.038 

d' 

30° 

1.03 

0.046 

K 

50° 

1.46 

0.065 

it 

60° 

1.86 

0.084 

t( 

65° 

2.17 

0.098 

C.o(I03)2+2H20 

0°, 

0.32. 

0.014 

ct 

18° 

0.45 

0.020 

(i 

30° 

0.52 

0.023 

i  '  f    .-      << 

50° 

0.67 

0.030 

<t 

75° 

0.84 

0.038 

<( 

100° 

1.02 

0.045 

Co(I03)2 

18° 

1.03 

0.046 

(i 

30° 

0.89 

0.040 

{( 

50° 

0.85 

0.036 

it 

75° 

0.75 

0.033 

14 

100° 

0.69 

0.031 

(Meusser,  B.  1901,  34.  2435.) 

+H2O.  Sol.  in  148  pts.  H2O  at  15°  and 
90  pts.  at  100°.  Sol.inNH4OH+Aq.  (Ram- 
melsberg, Pogg.  44.  561.)  ' 

Does  not  exist.  (Meusser,  B.  1901,  34. 
2434.) 

-f2H2O.    (Meusser.) 

+4H2O.    (Meusser.) 


404 


IODATE,  CUPRIC,  BASIC 


Cupric  iodate,  basic,  6CuO,  3I2O6+2H2O. 
Insol.  in  H2O.    (Millon,  A.  ch.  (3)  9.  400.) 
Mixture  of  CuO  and  Cu(IO«)2.     (Ditte, 

A.  ch.  (6)  21.  175.) 

2CuO,  I2O5+H2O.  Slowly  sol.  in  dil. 
H2SO4.  (Granger  and  de  Schulten,  Bull. 
Soc.  1904,  (3)  31.  1027.) 

Cupric  iodate,  Cu(IO3)2. 

1  1.  H2O  dissolves  3.32X10  3  mol.  Cu(IO3)2 
at  25°.  (Spencer,  Z.  phys.  Ch.  1913,  83. 
295.) 

Solubility  in  CuSO4+Aq  =  3.28X10  3  mol. 
per  1.  at  25°. 

Solubility  in  KIO3+Aq  =  3.29X10  3  mol. 
per  1.  at  25°.  (Spencer.) 

+H20.     (Ditte.) 

+2H2O.  Sol.  in  302  pts.  H2Q  at  15°,  and 
154  pts.  at  100°.  Sol.  in  HCl+Aq  or  NH4OH 
+Aq.  (Millon.) 

Cupric  iodate  ammonia,  Cu(IO3)2,  2NH3+ 

H20. 

Insol.  in  H2O.    (Ditte,  A.  ch.  (6)  21.  145.) 
Cu(IO3)2,  4NH3+2H2O.    Ppt.    (Ephraim, 

B.  19i5,  48.  52.) 

+3H2O.  Partially  sol.  in  H2O.  Sol.  in 
NH4OH+Aq.  Insol.  in  alcohol.  (Rammels- 

Cu(IO3)2,  5NH3.    (Ephraim.) 

Cu(IO3)2,8NH3+4H2O.  Sol.inH20.  Sol. 
in  NH4OH+Aq.  Insol.  in  alcohol.  (Ditte, 
A.  ch.  (6)  21. 145.) 

Decipium  iodate,  Dp(IO3)3+3H2O(?). 

Precipitate;  scarcely  sol.  in  H2O.  (Dela- 
fontaine.) 

Didymium  iodate,  Di(IO3)3+2H2O. 
Ppt.    (Cleve.) 

Erbium  iodate,  Er(IO3)3+3H2O. 
Very  si.  sol.  in  H2O.    (Hoglund.) 

Glucinum  iodate. 
Deliquescent. 

Indium  iodate,  In(IO3)3. 

1  pt.  is  sol.  in  1500  pts.  H2O  at  20°. 

1  pt.  is  sol.  in  150  pts.  HNO3  (1:5)  at  80°. 

Sol.  in  HC1  with  decomp.  Sol.  in  dil. 
H2SO4.  (Mathers,  J.  Am.  Chem.  Soc.  1908, 
30.  213.) 

Iodine  iodate,  I(IO3)3. 

Decomp.  by  H2O  or  by  alcohol.  (Fichter, 
Z.  anorg.  1915,  91.  142.) 

Iron  (ferrous)  iodate. 

Ppt.  SI.  sol.  in  H2O;  more  sol.  in  FeSO4  + 
Aq.  (Geiger,  Mag.  Pharm.  29.  252.) 


Iron  (ferric)  iodate,  Fe2O3,  I2O5. 

Insol.  in  acids.    (Ditte,  A.  ch.  (6)  21.  145.) 
Fe2O3,  2I2O5+8H2O.    Sol.  in  500  pts.  H2O. 

Difficultly  sol.  in  HN O3  +  Aq.    Sol.  in  FeCl3  + 

Aq.     (Geiger.) 

3Fe2O3,   5I2O5+15H2O.  .  Sol.  in  HC1,   or 

HNO3+Aq.    (Rammelsberg.) 

Lanthanum  iodate,  La(IO3)3  +  13/£E2O. 

SI.  sol.  in  cold,  easily  sol.  in  hot  H2O. 
Very  sol.  in  warm  HCl+Aq.  (Holzmann,  J. 
pr.  76.  349.) 

100  cc.  of  the  sat.  solution  in  H2O  contain 
0.1681  g.  at  25°.  (Rimbach,  Z.  phys.  Ch. 
1909,  67.  199.) 

Calc.  from  electrical  conductivity  of 
La(IO3)3+Aq,  100  cc.  of  the  sat.  solution 
contain  0.1871  g.  La(IO3)3  at  25°.  (Rim- 
bach.) 

Lead  iodate,  basic,  3PbO,  Pb(IO3)2+2H2O. 
Ppt.    (Stromholm,  Z.  anorg.  1904,  38.  442.) 

Lead  iodate,  Pb(I03)2. 

Very  si.  sol.  in  H2O  (Pleischl),  and  dif- 
ficultly sol.  in  HNO3+Aq.  (Rammelsberg.) 

Insol.  inH2O  and  H2SO4+Aq.  Very  si. 
sol.  in  HNO3+Aq,  and  wholly  insol.  therein 
after  being  heated  to  100°.  (Ditte,  A.  ch. 
(6)  21.  169.) 

SI.  sol.  in  H2O.  1.83  X  10~2  are  dissolved  in 
1  liter  of  sat.  solution  at  20°.  (Bottger,  Z. 
phys.  Ch.  1903,  46.  603.) 

1  1.  H2O  dissolves  19  mg.  Pb(IO3)2  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1904,  50.  356.) 

17.8  mg.  are  dissolved  in  1  1.  sat.  solution 
at  18°.  (Kohlrausch,  Z.  phys.  Ch.  1908,  64. 
168.) 

1  1.  H2O  dissolves  0.0307  g.  Pb(IO3)2  at 
25°.  (Harkins,  J.  Am.  Chem.  Soc.  1911,  33. 
1830.) 

Solubility  of  Pb(IO3)2  in  salts +Aq  at  25°. 

C  =  concentration  of  salt  in  salt  solution 
expressed  in  equivalents  per  1. 

S  =  solubility  of  Pb(IO3)2  in  salt  solution 
expressed  in  equivalents  per  1. 


Salt 

C 

s 

Pb(N03)2 

0.0001 
0.001 
0.010 
0.100 
0.500 
3.0 

0.0000870 
0.0000411 
0.0000185 
0.000016 
0.000028 
0.000015 

KNO3 

0.002 
0.010 
0.050 
0.200 

0.0001141 
0.0001334 
0.0002037 
0.0002544 

KI03 

0.00005304 
0.0001061 

0.0000697 
0.0000437 

(Harkins  and  Winninghof,  J.  Am.  Chem.  Soc. 
1911,  33.  1830.) 


IODATE,  POTASSIUM 


405 


Insol.  in  liquid  NH3.     (Gore,  Am.  Ch.  J 
1898,  20.  828.) 


Lithium  iodate, 

Deliquescent,  and  very  sol.  in  H2O. 

Sol.  in  2  pts.  cold,  and  not  much  less  hot 
H2O.  Insol.  in  alcohol.  (Rammelsberg, 
Pogg.  44.  555.) 

Sp.  gr.  of  solution  sat.  at  18°  =  1.568,  con- 
taining 44.6%  LiIO3.  100  g.  H2O  dissolve 
80.3  pts.  LiIO3.  (Mylius  and  Funk,  B.  1897, 
30.  1718.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

+H2O.  Very  deliquescent.  (Ditte,  A.  ch. 
(6)  21.  145.) 

Magnesium  iodate,  Mg(IO3)2. 

Anhydrous.     Insol.  in  H2O.     (Millon,  A. 

ch.  (3)  9.  422.) 

+4H2O.    Very  sol.  in  H2O.    (Ditte.) 
Sol.  in  9.43  pts.  H2O  at  15°,  and  3.04  pts. 
100°.     (Berzelius.)     Very  si.  sol.  in  H2O. 


at          .  . 

(Serullas,  A.  ch.  45.  279.) 
H2SO4+Aq.    (Ditte.) 


.       . 
Easily  sol.  in  dil. 


0° 

6.8 

35° 

8.9 


Sat.  solution  contains  at: 
10°      20° 

6.4      7.7%Mg(I03)2, 

63°      100° 

12.6     19.3%Mg(IO3)2. 


(Mylius  and  Funk,  B.  1897,  30.  1722.) 

Sat.  aq.  solution  at  18°  contains  6.44% 
Mg(IO3)2  or  6.88  g.  are  sol.  in  100  g.  H2O. 
Sp.  gr.  of  sat.  solution  =  1.078.  (Mylius  and 
Funk,  B.  1897,  30.  1718.) 

+  10H2O.     Sat.  aq.  solution  contains  at: 
0°      20°       30°       35°       50°(m.pt.). 
3.1    10.2     17.4     21.9     67.5%  Mg(IO3)2. 
(Mylius  and  Funk,  B.  1897,  30.  1723.) 

Manganous  iodate,  Mn(IO3)2-fH2O. 

Sol.  in  about  200  pts.  H2O.  (Rammels- 
berg.) 

Insol.  in  H2O  and  HNO3-f-Aq,  even  on 
boiling.  Insol.  in  NH4OH+Aa.  (Ditte.) 

Manganous  manganic  iodate, 

Mn(I03)4,  Mn(I03)2. 
Insol.  in  H2O.     (Berg,  C.  R.  1899,  128. 

675.) 

Manganic  potassium  iodate, 

Mn(IO3)4,  2KIO3. 

Insol.  in  and  only  si.  attacked  by  H2O. 
Insol.  in  HIO3.     (Berg,  C.  R.  1899,  128. 

674.) 

Mercurous  iodate,  Hg2(IO3)2. 

Insol.  in  boiling  H2O,  or  cold  HNO3+Aq. 
Easily  sol.  in  dil.  HCl+Aq.  Sol.  in  very 


cone.  HIO3+Aq.     (Lefort,  J.  Pharm.  1845. 

5.) 

Mercuric  iodate,  Hg(IO3)2. 

Insol.  in  H2O  or  alcohol.  (Millon,  A.  ch. 
(3)  18.  367.)  Sol.  in  H2O.  (Berzelius.)  Sol. 
in  dil.  HCl+Aq.  (Rammelsberg.) 

Nearly  insol.  in  H2O.  Easily  sol.  in  HC1, 
HBr,  or  HI+Aq;  very  si.  sol.  in  HNO3+Aq; 
insol.  in  HF,  H2SiF6,  or  HC2H3O2+Aq.  Sol. 
in  alkali  chlorides,  bromides,  iodides,  cy- 
anides, and  cyanates+Aq;  also  in  Na2S2O3, 
dil.  MnCl2,  and  ZnCl2+Aq.  Insol.  in  KOH, 
NaOH,  NH4OH,  Na2S,  Na2B4O7,  Na2HPO4, 
and  the  alkali  chlorates,  bromates,  and  iodates 
-f  Aq.  (Cameron,  C.  N.  33.  253.) 

Nickel  iodate,  Ni(IO3)2. 

Solubility  in  H2O. 


Form 

Temp. 

Percent  oj 
Ni(IOs)2 
in  solu- 
tion 

Mols.  water 
free  salt  to 
100  mols. 
H20 

Ni(IO?)2+4H20 

0° 

0.73 

0.033 

a 

18° 

1.01 

0.045 

(i 

30° 

1.41 

0.063 

<zNi(I03)2+2H20 

0° 

0.53 

0.023 

(i 

18° 

0.68 

'  0.030 

it 

30° 

0.86 

0.039 

« 

50° 

1.78 

0.080 

/3Ni(I03)2+2H20 

8° 

0.52 

0.023 

ii 

18° 

0.55 

0.0245 

<( 

50° 

0.81 

0.035 

(i 

75° 

1.03 

0.045 

(( 

100° 

1.12 

0.049 

Ni(I03)2 

30° 

1.135 

0.050 

11 

50° 

1.07 

0.046 

<i 

75° 

1.02 

0.045 

(i 

100° 

0.988 

0.044 

(Meusser,  B.  1901,  34.  2440.) 

+H2O.  Sol.  in  120.3  pts.  H2O  at  15°,  and 
77.35  pts.  at  100°.  (Rammelsberg,  Pogg. 
44.  562.) 

Sol.    in    HNO3,    and    dil.    H2SO4+Aq. 
(Ditte.) 

Sol.  in  NH4OH+Aq. 

Does  not  exist  (Meusser.) 

+2H2O.    See  Meusser  above. 

+3H2O.  Insol.  in  H2O.  Sol.  in  HNOS. 
(Ditte,  A.  ch.  1890,  (6)  21.  160.) 

+4H2O.    See  Meusser  above. 

Nickel  iodate  ammonia,  Ni(IO3)2,  4NH8. 

Sol.  in  NH4OH+Aq.  Insol.  in  alcohol. 
(Rammelsberg,  Pogg.  44.  562.) 

Ni(IO3)2,  5NH8.  Ppt.  (Ephraim,  B.  1915, 
48.  53.) 

+3H2O.    (Ephraim.) 

Potassium  iodate,  KIO3. 

1  pt.  KIO3  dissolves  in  13  pts.  H2O  at  14°. 
(Gay-Lussac.) 


406 


IODATE,  POTASSIUM  HYDROGEN 


1  pt..KIO3  dissolves  at: 
0°  in  21.  11  pts. 
20°  "  12.29 
40°"     7.76 
60°  "     5.40 
80°"     4.02 
100°"     3.10 

Sat.    solution    boils    at    If 

H2O 

12°        CKrpmprs 

Sol.  in  75  pts.     H2O   at   15°.     Insol.   in 
alcohol.    (Serullas,  A.  ch.  22.  181.) 
See  also  Meerburg  under  KIO3. 

Potassium    c&hydrogen    io.date,    KH2(IO3)2. 
Sol.  in  25  pts.  H2O  at  15°.    (Serullas,  A.  ch. 
43.  117.) 
See  also  Meerburg  under  KIO3. 

Pogg.  97.  5.) 

Sp.  gr.  of  KIO3+Aq  containing: 

1  2  3  4  5        %KI03, 

1.010   1.019    1.027    1.035   1.044 

6  7  8  9         10       %KIO3. 

1.052    1.061    1.071    1.080  1.090 
(Kremers,  Pogg.  96.  62.) 

Stable  at  10°  in  H2O  or  potassium  acetate 
+Aq.    (Eakle,  C.  C.  1896,  II.  649.) 

Solubility  of  KIO3  in  HIO3+Aq  at  30°. 


More  sol.  in  KI+Aq  than  in  H2O.  Sol.  in 
warm  H^SO-iH-Aq. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Insol.  in  alcohol. 

Insol.  in  methyl,  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,  43  314.) 

(Ditte,C.R.70.621.) 


Potassium  hydrogen,  iodate,  KH(IO3)2. 

Sol.  in  18.65  pts.  H2O  at  17°.    (Meineke,  A. 
261.  360.) 


Potassium  tellurium  iodate. 
See  lodotellurate,  potassium. 

Potassium  uranyl  iodate, 
,KU02(IO3)3+3H2O. 

Decomp.  by  H2O,  dil.  salt  solutions  and 
UO2(NO3)2+Aq.  (Artmann,  Z.  anorg.  1913. 
79.  340.) 

Potassium  iodate  chloride,  KH(I03)2,  2KC1.' 
Sol.  in  19  pts.  H2O  at  15°  with  decomp. 


%  HI03 

%  KIO3 

L/oia  aiconoi  dissolves  out  ivvjl. 

.  in  .the 

in.  the 

Solid  phase 

solution 

solution 

Potassium  iodate  molybdate,  KIO3,  MoO3  + 

OTT    ^~\ 

0 

0.64 

9.51 
9.48 

KI03 
KI03+KI03,  HI03 

2H2O. 
See  Molybdatoiodate,  potassium. 

0  66 

.9.52 

u 

0^65 

9^46 

u 

Potassium  iodate  selenate. 

0.65 

8.90 

KIO3,  HIO3 

See  lodoselenate,  potassium. 

0.67 

6.6 

" 

1.14 

4.57 

" 

Potassium  iodate  sulphate,  K1O3  KHSO4. 

1.69 
2.02 

3.63 
3.10 

u 

Decomp.  by  H2O.    (Marignac,  J.  B.  1856. 
299.) 

3.34 

5f\f\ 

2.14 

1or> 

11 

KHIO3,  KHSO4.    More  sol.  in  H2O  than 

.00 
7.09 

.32 
1.0   ' 

u 

KHIO3.    (Serullas.) 

8.04 
3.47 

0.85 
3.57 

KIO3HIO3+KIO3,  2HIO3 
KIO3,  2HIO3  (labile) 

Potassium  iodate  tungstate. 

4.80 

2.90 

u 

See  Tungstoiodate,  potassium. 

6.45 

1.35 

" 

9.35 

0.64 

KI03,  2HIO3 

Rubidium  iodate,  RbIO3. 

12.04 
17.50 
31.20. 

0.44 
0.30 
0.52 

a 
n 

100  pts.  HsO  dissolve  2.1  pts.  RbIO3  at 
23°.    Easily  sol.  in  cold  HCl+Aq.    (Wheeler 
Sill.  Am.  J.  144.  123.) 

53.64 

0.68 

11 

62.52 
76.40 

0.72 
0.80 

KI03,  2HIO3+HI03 

Rubidium  hydrogen  iodate,  RbH(IO3)2. 

76.70 

0 

HIO3 

SI.  sol.  in  cold,  more  readily  in  hot  H2O, 

RbIO3  separating  on  coolins     Insol  in  alco- 

(Meerburg,  Z.  anorg.  1905,  46.  330.) 

hoi.     (Wheeler.) 

-     '. 

RbH2(IO3)3.     As  above.     (Wheeler.) 

Rubidium  iodate  chloride,  RbIO3,  HC1,  or 

HI03,  RbCl. 

Decomp.  by  cold  H2O.    (Wheeler.) 
3RbCl,  2HIO3.     Sol.  in  H2O,  from  which 

RbIO3  separates.    (Wheeler.) 

Rubidium  iodate  selenate. 
See  lodoselenate,  rubidium. 

Samarium  iodate,  Sm(IO3)3-f;6H2O. 
Precipitate.     (Cleve.) 


IODATE  IODIDE,  SODIUM 


407 


Scandium  iodate,  Sc(IO3)3  +  10,  13,  15,  and 

18H20. 

Nearly    insol.    in    H2O.      (Crookes,    Phil. 
Trans.  1910,  210.  A,  361.) 


(Hill  and  Simmons,  Z.  phys.  Ch.  1909,  67. 
602.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  829.) 

Insol.  in  methyl  acetate.  (Bezold,  Dis- 
sert. 1906;  Naumann,  B.  1909,  42.  3790); 
ethyl  acetate.  (Hamers,  Dissert.  1906; 
Naumann,  B.  1910,  43.  314.) 

Silver    iodate    ammonia,    2AgIO3,    3NH3  + 


Very  sol.  in  cold  H2O.  (Ditte,  A.  ch.  (6) 
21.  145.) 

AgIO3,  2NH3. 

SI.  sol.  in  cone.  NH4OH+Aq.  (Rosen- 
heim,  A.  1899,  308.  52.) 

Sodium  iodate,  NaIO3. 

ICO  pts.  H2O  dissolve  7.25  pts.  NaIO3  at 
14.5°.  (Gay-Lussac.)  100  pts.  H2O  dissolve 
2.52  pts.  at  0°;  9.07  pts.  at  20°;  14.39  pts.  at 
60°;  27.7  pts.  at  80°;  33.9  pts.  at  100°.  (Krem- 


ers,  Pogg.  97.  5.)    Sat.  solution  boils  at  102° 
(Kremers),  105°  (Ditte). 

Sol.  in  warm  H2SO4+Aq  diluted  with  Y* 
vol.  H2O.  Crystallizes  out  on  standing  over 
H2S04.  (Ditte.) 


Silver  iodate,  AgIO3. 
189XlO~4  moles  or  5.36X10~2  g.  AgIO3 

Solubility  of  NaIO3  in  HIO3+Aq  at  30°. 

are  sol.  in  1  liter  H2O  at  25°.     (Noyes  and 

%  HI03 

%  NalOs 

Kohr,  Z.  phys.  Ch.  1903,  42.  338.) 
SI.  sol.  in  H2O.    4.35X10-2  g.  are  dissolved 

in  the 
solution 

in  the 
solution 

Solid  phase 

in  1  liter  of  sat.  solution  at  20°.    (Bbttger,  Z. 

o 

9  .  36 

NaIO3+l/^H2O 

phys.  Ch.  1903,  46.  603.) 

1.98 

9.52 

1  1.  H2O  dissolves 

40  mg.  AgIO3  at  18°. 

4!  86 

10.22 

t 

(Kohlrausch,  Z.  phys. 

Ch.  1904,  50.  356.) 

5^86 

11.04 

i 

1  1.  H2O  dissolves  0.0275  g.  AgIO3  at  9.43°; 

7.40 

11.60 

'         ll    U'l 

0.039  g.  at  184°;  0.0539  g.  at  26.6°.     Solu- 

9*73 

14.73 

«      [labile 

bility  increases  rapidly  with  temp.     (Kohl- 

6^76 

11.18 

NaIO3+l^H2O  + 

rausch,  Z.  phvs.  Ch.  1908,  64.  168.) 
1  1.  H2O  dissolves  0.039  g.  AgIO3  at  20°. 

6.66 

11.28 

Na2O,  2I206 

(Whitby,  Z.  anorg.  1910,  67.  108.) 
Not  completely  insol.  in  H2O.    (Rose.)  Sol. 

7^80 
9.15 

10^30 
9.00 

Na2O,  2I2O6 

u 

in  NH4OH+Aq;  sol. 

in  HNO3+Aq.     (Na- 

9.93 

8.71 

n 

quet,  J.  B.  1860.  201.) 

Sol.  in  cone.  KI+Aq. 

11  20 

7  54 

a 

(Ladenburg,  A.  135.  1.) 
Sol.  in  27,700  pts.  H2O  at  25°;  in  42.4  pts. 

11.89 
11.75 

7.21 

7.18 

Na20,  2I2O5-f  NaIO3,  2HIO8 

5%  NH4OH+Aq  at 

25°;  in  2.1  pts.   10% 

14.62 

5.65 

NalO    2HlOs 

NH4OH+Aq   at  25°;   in    1044.3   pts.   35% 

23.23 

3.69 

•    a 

HNO3+Aq   (sp.  gr.   1.21)   at  25°.     (Longi, 

32.68 

2.91 

(i 

Gazz.  ch.  it.  13.  87.) 

40.  9l 

2.64 

tt 

46  62 

2  67 

(i 

Solubility  in  HNO3+Aq  at  25°. 

55.48 

2.12 

tt 

Normality  HNOs 

G.  AglOs  dissolved  per  1. 

65.47 
76.19 

1.83 
1.42 

NaIO3,  2HIO3+HIO3 

0.000 

0.0503 

76.70 

0 

HI03 

0,125 
0.250 

0.0864 
0.1075 

(Meerburg,  Z.  anorg.  1905,  45.  334.) 

0.500 
1.00 

0.1414 
0.2067 

Insol.  in  alcohol.    Sol.  in  dil.  HC2H8O2+ 

2.00 

400 

0.3319 

q- 

Insol.  in  methyl  acetate.     (Naumann,  B. 

.  uu 

IK  O^  K 

1909,42.3790.) 

8.00 

.5875 

+13^H2O.     See  Meerburg  above. 

Sodium  duodate,  Na2O,  2I2O6. 
See  Meerburg  under  NaIO3. 


Sodium  Zniodate,  NaIO3, 

Very  sol.  in  H2O.    (Blomstrand,  J.  pr.  (2) 
42.  337.) 

See  also  Meerburg  under  NaIO3. 

Sodium  iodate   bromide,   NaIO3,   2NaBr+ 

9H20. 
Sol.  in  H2O.    (Rammelsberg.) 

Sodium  iodate  chloride,  NaIO8,  NaCl+4H2O, 

and  2NaIO3,  3NaCl+18H2O. 
Cold  H2O  dissolves  out  NaCl.  . 

Sodium  iodate  iodide,  NaIO3,  Nal. 

Hot  H2O  or  alcohol  dissolves  out  Nal. 

+8H2O. 

+  10H2O. 

2NaIO3,   3NaI+20H2O.     (Penny,  A.  37. 
202.) 


408 


IODATE,  STRONTIUM 


Stable  in  a  solution  of  Nal+NaOH+Aq. 
(Eakle,  C.  C.  1896,  II.  650.) 

Strontium  iodate,  Sr(IO3)2. 

Anhydrous.  Insol.  in  H2SO4  (Ditte);  easily 
sol.  in  cold  HCl+Aq.  (Rammelsberg.  Pogg. 
44.  575.) 

+H2O.    Difficultly  sol.  in  H2O. 

+6H2O.  Sol.  in  416  pts.  H2O  at  15°,  and 
138  pts.  at  100°  (Gay-Lussac);  342  pts.  at  15°, 
and  110  pts.  at  100°.  Difficultly  sol.  in  warm 
HNO3+Aq.  (Rammelsberg,  Pogg.  44.  575.) 

Thallous  iodate,  T1IO3. 

Difficultly  sol.  in  warm  H2O.    (Oettinger.) 

Insol.  in  H2O;  difficultly  sol.  in  HNO3+Aq. 
(Rammelsberg.) 

SI.  sol.  in  H2O. 

0.58  X10-1  g.  are  dissolved  in  1  liter  of  sat. 
solution  at  20°.  (Bottger,  Z.  phys.  Ch.  1903, 
46.  603.) 

2.12X10-3  mols.  =0.667  g.  are  sol.  in  1  1. 
H2O  at  25°.  (Spencer,  Z.  phys.  Ch.  1912,  80. 
707.) 

Sol.  in  a  little  NH4OH+Aq,  also  in  boiling 
HNO3,  H2SO4,  or.  HC1  +  Aq.  Insol.  in  alcohol. 
(Oettinger.) 

+  i^H2O.  Very  si.  sol.  in  H2O  or  dil.  boil- 
ing acids.  (Ditte,  A.  ch.  (6)  21.  145.) 

Thallic  iodate,  basic,  T1(OH)(IO3)2+H2O  = 

T12O3,  2I2O6+3H2O. 

Insol.  in  H2O;  sol.  in  cold  HCl+Aq,  and 
warm  dil.  H2SO4+Aq.  (Ditte,  A.  ch.  (6)  21. 
145.) 


Thallic  iodate,  T1(IO,),+1^  H2O. 

Insol.  in  H2O;  si.  sol.  in  HNO3+Aq. 
Decomp.  by  alkalies.  (Rammelsberg.) 

+12H2O.    Difficultly  sol.  in  H2O. 

Easily  sol.  in  dil.  acids.  (Gewecke,  Z. 
anorg.  1912,  76,  275.) 

Thorium  iodate,  Th(IO3)4. 
Precipitate.    (Cleve.) 

Tin  (stannous)  iodate. 

Ppt.  Sol.  in  SnCl2+Aq;  insol.  in  NaIO3+ 
Aq. 

Tin  (stannic)  iodate. 
Ppt. 

Uranous  iodate. 

Precipitate.  Very  unstable.  (Rammels- 
berg.) 

Uranyl  iodate,  UO2(IO3)2. 

Sol.  or  insol.  in  HNO3  and  H3PO4+Aq, 
according  to  method  of  preparation.  (Ditte.) 

+H2O.  Sl.sol.inHNO3+Aq.  (Rammels- 
berg.) 


Ytterbium  iodate,  Yb(IO3)3+6H2O. 

Ppt.     (Cleve,  Z.  anorg.  1902,  32.  136.) 

Yttrium  iodate,  Y(IO3)3+3H2O. 
Sol.  in  190  pts.  H2O.    (Berlin.) 

Zinc  iodate,  Zn(IO3)2. 

Anhydrous.     (Ditte,  A.  ch.   (6)  21.  145.) 

+2H2O.  Sol.  in  114  pts.  cold,  and  76  pts. 
hot  H2O.  (Rammelsberg,  Pogg.  43.  665.) 

Sol.  in  HNO3,  and  NH4OH+Aq. 

Exists  also  in  a  very  sol.  modification. 
(Mylius  and  Funk,  B.  1897,  30.  1723.) 

Zinc  iodate  ammonia,  3ZndO3)2,  8NH3. 

Decomp.  by  H2O;  sol.  in  NH4OH+Aq, 
from  which  it  is  pptd.  by  alcohol.  (Rammels- 
berg, Pogg.  44.  563.) 

Zn(IO3)2,  2NH3.  Insol.  in  H2O.  (Ditte,  A. 
ch.  (6)  21.  145.) 

Zn(IO3)2,  3NH3+H2O.  Insol.  in  H2O. 
(Ditte.) 

Zn(IO3)2,  4NH3.  (Ditte,  A.  ch.  1890,  (6) 
21.  1Q4.)  (Ephraim,  B.  1915,  48.  53.) 

Periodic  acid. 
See  Periodic  acid. 

Iodides. 

The  iodides  are  in  general  easily  sol.  in 
H2O;  exceptions  are  HgI2,  PbI2,  Agl,  Cu2I2, 
and  BiI3,  also  the  iodides  of  the  Pt  metals, 
all  of  which  are  insol.  SnI4,  SbI3,  and  T1I3  are 
decomp.  by  H2O.  Many  iodides  are  more  sol. 
in  solutions  of  salts  than  in  H2O,  and  several 
are  sol.  in  alcohol  or  ether. 

See  under  each  element. 

Iodine,  I2. 

Sol.  in  5524  pts.  H2O  at  0-12°.  (Wittstein,  J.  B. 
1857.  123.) 

Sol.  in  7000  pts.  H2O.     (Gay-Lussac.) 
Sol.  in  3800  pts.  H2O  at  15°.     (Basse.) 
Sol.  in  500  pts.  H2O.     (Jacquelain.) 
Sol.  in  7196.4  pts.  B2O  at  18.75.     (Abl.) 

Pure  H2O  dissolves  0.01519173  g.  I  per 
litre,  or  I  is  sol.  in  6582  pts.  H2O  at  6.3°. 
(Dossius  and  Weith,  Zeit.  Ch.  12.  378.) 

Sol.  in  about  4500  pts.  H2O.  (Hager, 
Comm.  1883.) 

Sol.  in  7000  pts.  H2O.  (Cap  and  Garot,  J. 
Pharm.  (3)  26.  80.) 

1  1.  H2O  at  25°  dissolves  0.3387  g.  I2. 
(Jakowkin,  Z.  phys.  Ch.  1895,  18.  590.) 

1 1.  H2O  dissolves  1.342  millimols  of  iodine 
at  25°.  (Noyes,  Z.  phys.  Ch.  1898,  27.  359.) 

When  iodine  is  shaken  with  H2O  at  15°,  1 
pt.  dissolves  in  3750  pts.  H2O;  when  iodine 
and  H2O  are  heated  together  and  then  cooled 
to  15°,  1  pt.  iodine  dissolves  in  3500  pts.  H2O. 

At  30*,  1  pt.  is  sol.  in  2200  pts.  H2O. 
(Dietz,  Chem.  Soc.  1899,  76,  (2)  150.) 

1  1.  H2O  dissolves  0.279  grams  I2  at  25°. 
(McLauchlan,  Z.  phys.  Ch.  1903,  44.  617.) 


IODINE 


409 


Solubility  of  I2  in  H2O  at  t°. 

Solubility  hi  HgCl2+Aq  at  25°. 

t°                                     g.  I2  per  1.  H20 

10  ccm.  of  the  solution  contain: 

18                                0.2765 
25                                0.3395 
35.                              0.4661 
45                                0.6474 
55                                0.9222 

millimols  1  2                              millimols  Hg 

0.0134                          0 
0.1294                          0.9444 
0.1460                           1.2442 
0.1806                           1.9542 
0.2543                          3.3460 

(Hartley,  Chem.  Soc.  1908,  93.  744.) 
Solubility  of  I2  in  H2O  at  t°. 

(Herz  and  Paul,  Z.  anorg.  1914,  85.  214.) 

Sol.  in  solutions  of  soluble  iodides. 
100  pts.  KI+200  pts.  H2O  dissolve  153 
pts.  I;  from  this  solution  H2O  precipitates  % 
the  dissolved  I.     100  pts.  KI+400  pts.  H2O 
dissolve  quickly  76.5  pts.  I.     If  more  water 
is  present,    the  solution   takes  place  more 
slowly.     (Baup.) 
CS2  extracts  the  I  from  the  above  solutions. 

Solubility  of  I  in  KI+Aq  at  7-7.3°. 

t°                     g.  per  1.                       milliat.  per  1. 

0               0.1649                     1.30 
20              0.2941                    2.30 
40               0.5684                     4.56 

(Fedotieff,  Z.  anorg.  1910,  69.  30.) 

1.32  millimol  I2  are  sol.  in  1  1.  H2O.    (Bray' 
J.  Am.  Chem.  Soc.,  1910,  32.  938.) 
Calculated  from  electrical  conductivity  of 
sat.  I2+Aq.  1  1.  H2O  dissolves  0.0006383  mols. 
I2  at  0°.    (Jones,  J.  Am.  Chem.  Soc.  1915,  37. 
256.) 
Cone.    H2S04,    HC1,    HNO3,    H3PO4, 
HC2H3O2,  tartaric,  or  citric  acids  +Aq  dis- 
solve I,  but  give  it  up  to  CS2  on  shaking 
therewith.    (Tessier,  Z.  anal.  11.  313.) 
Sol.  in  150  pts.  H2SO4  on  warming,  but 
crystallizes  out  in  part  on  cooling.    (Kraus.) 
Much  more  sol.  in  HBr+Aq  than  in  pure 
H2O;   HBr+Aq   of  sp.   gr.    1.486   dissolves 
3-4%.     (Bineau.) 
SI.  sol.  in  HCl+Aq.    Easily  sol.  in  even 
dil.  HI+Aq. 
1  1.  0.001  N-HCl+Aq  sat.  with  I2  contains 
0.338  g.  I2.    (Bray  and  Mackay,  J.  Am.  Chem. 
Soc.  1910,  32.  1919.) 

%  KI  in  KI  +Aq 

Pts  I  dissolved 

Sp.  gr.  of  solution 

1.802 
3.159 
4.628 
5.935 
7.201 
8.663 
10.036 
11.034 
11.893 
12.643 

1.173 
2.303 
3.643 

4.778 
6.037 
7.368 
8.877 
9.949 
11.182 
12.060 

1.0234 
1.0433 
1.0668 
1.0881 
1.1112 
1.1382 
1.1637 
1.1893 
1.2110 
1.2293 

1  1.  0.1  N—  HNO3+Aq  sat.  with  I2  contains 
0.340  g.  I2.    (Sammet,  Z.  phys.  Ch.  1905,  53. 
644.) 
1  1.  0.1  N-H2SO4+Aq  sat.  with  I2  contains 
0.341  g.  I2.    (Sammet.) 
Sol.  in  H2SO3+Aq  with  decomp. 
1  1.  0.9  N.  H3BO3  dissolves  0.300  g.  I2  at 
25°.     (McLauchlan,  Z.  phys.  Ch.  1903,  44. 
617.) 
100  cc.  of  a  10%  solution  of  BaBr2  dis- 
solve 0.231  g.  I2  at  13.5°.     (Meyer,  Z.  anorg. 
1902,  30.  114.) 
100  cc.  of  a  10%  solution  of  BaCl2  dissolve 
0.067g.  I2  at  18.5°.    (Meyer.) 
100  cc.  of  a  10%  solution  of  BaI2  dissolve 
6.541  g.  I2  at  13.5.°     (Meyer.) 
100  cc.  of  a  10%  solution  of  CaBr2  dis- 
solve 0.274  g.  I2  at  13.5.°    (Meyer.) 
100  cc.  of  a  10%  solution  of  CaCl2  dissolve 
0.078  g.  I2  at  18.5°    (Meyer.) 
100  cc.  of  a  10%  solution  of  CaI2  dissolve 
8.062  g.  I2  at  13.5°.    (Meyer.) 
Easily    sol.    in    boiling    dil.    HgCl2+Aq. 
(Selmi.) 

(Dossius  and  Weith,  Zeit.  Ch.  (2)  6.  379.) 

Solubility  of  I2  in  KI+Aq  at  room  tempera- 
ture, 14.5°-15.1°. 

%  KI 

%I 

I/KI 

1.80 
3.16 
4.63 
5.93 
7.20 
8.66 
10.04 
11.03 
11.89 
12.64 

1.17 
2.30 
3.64 
4.78 
6.04 
7.37 
8.88 
9.95 
11.18 
12.06 

0.651 
0.729 
0.786 
0.805 
0.839 
0.851 
0.884 
0.902 
0.940 
0.954 

(Weith  and  Dossius,  Z.  phys.  Ch.  1898,  26. 
150.) 

410 


IODINE 


S.olubility  of  I2  in  KI+Aq  at  15° 

Solubility  in  KI+Aq  at  25°. 

%  KI 

ccm.  1/10-n.  iodine  in 
5cmm.  of  the  solution 

I/KI 

Sp.  gr. 

Analysis  of  liquid 
phase 

Analysis  of  solid 
phase  together  with 
adhering  mother 
liquor 

10 

8 
6 
4 
2 
1 

35.0 
27.1 
19.7 
12.7 
6.25 
3.04* 

35.0 
.  33.9 
32.8 
31.8 
31.2 
30.4 

%  KI 

%i 

'%  KI     |       %  I 

(a) 

1.733 

1.888 
2.066 
2.216 
2.539 
2.560 
2.665 
3.232 
3.246 

(b) 

1.349 
1.516 
1  .  769 
1.910 
2.403 
2.904 
3.082 

(c)  In\ 
3.316 

[n  equilib 

60.39 
54.415 
49.045 
44.82 
38.065 
37.655 
35.805 
29.71 
27.92 

In  equili 

16.025 
19.705 

22.88 
23,55 
24.78 
24.995 
25.18 

'-ariant  po 

26.05 
25.96 
26.04 
25.92 

rium  with 

0.0 
11.63 
23.085 
31.01 
44.56 
45.55 
49.61 
62.81 
66.45 

Drium  wit 

18.49 
26.16 
36.06 
40.515 
53  .  605 
63  .  125 
66.04 

int.    Exc( 

68.06 
68.01 
68.16 
68.13 

excess  o 

84.92 
85.94 
80.46 
78.56 
77.32 

39.99 

38.78 

i  excess 

3.04 

4.48 
3.70 
6.49 
8.62 
4.82 
4.00 

iss  of  KI 

16.14 
11.32 

f  KI. 

0.0 
4.05 
6.32 
10.84 
15.23 
16.73 

56.10 

56.27 

of  I. 

85.43 
83.87 
89.33 
83.62 
83.81 
92.41 
94.39 

and  I. 

83.77 
86.56 

*  Obtained  with  1/100-normal  iodine. 
(Brunei,  Z.  phys.  Ch.  1898,  26.  151.) 

Solubility  of  I2  in  KI+Aq  at  25°. 

Millimols  KI  per  liter 

Millimols  dissolved  iodine 
per  liter 

106.3 
53.15 
26.57 
13.29 
6.643 
3.322 
1.661 
0.8304 

55.28 
28.03 
14.68 
8.003 
4.667 
3.052 
2.235 
1.814 

(Noyes  and  Seidenstricker,  Z.  phys.  Ch.  1898, 
27.  359.) 

Solubility  in  KI+Aq  at  25°, 


(Parsons  and  Whittemore,  J.  Am.  Chem. 
1911,  33.  1934.) 

Solubility  in  KI+Aq  at  0°. 


KI    mol./l. 

I    G.  atoms/1. 

1.91 

2.85 
4.51 
5.36 
5.55 

3.29 
5.45 
11.52 
17.12 
17.16 

(Abegg,  Z.  anorg.  1906,  50.  427.) 


Solubility  of  I2  in  KI+Aq  at  25°, 


Millimol  KI  per  1. 

Millimol  1  2  dissolved 

100 

51.35 

50 

25.77 

20 

11.13 

10 

6.185 

5 

3.728 

2 

2.266 

1 

1.788 

(Bray  and  MacKay,  J.  Am.  Chem.  Soc.  1910, 
32.  919.) 


KI+Aq 

KI+Aq.  sat.  with  I2 

Wt.  norm. 

Sp.  gr.  0°/4° 

G.  I2  in  1  g. 
of  solution 

Sp.  gr.  0°/4° 

0.09871 

(1.0123) 

0.01199 

(1.0219) 

0.09861 

1.01231 

0.01199 

1.02187 

0.04969 

(1.0061) 

0.006094 

(1.0109) 

0.04966 

1.00610 

0.006083 

1.01089 

0.01992 

1.00236 

0.002535 

1.00429 

0.01983 

(1.0024) 

0.0025325 

(1.0044) 

0.00998 

(1.0011) 

0.0013532 

(1.0020) 

0.00992 

(1.001.1) 

0.0013585 

(1.0020) 

0.004999 

(1.0005) 

0.0007609 

(1.0010) 

0.004991 

(1.0005) 

0.0007577 

(1.0011) 

0.002000 

(1.0001) 

0.0004137 

(1.0004) 

0.002000 

(1.0001) 

0.0004015 

(1.0004) 

0.000999 

(0.9999) 

0.0002839 

(1.0002) 

0.000992 

(1.0000) 

0.00028125 

(1.0002) 

Values  in  parentheses  are  found  by  inter- 

polation. 

(Jones  and  Hartman,  J.  Am.  Ghem.  Soc.  1915, 

37.  247.) 

1  mol.  KI  in  alcohol  dissolves  2  atoms  I, 

and  the  solution  does  not  give  up  I  to  CS2. 

(Jorgensen,  J.  pr.  (2)  2.  347.) 

IODINE 


411 


Solubility  in  KI+60%  alcohol  at  25°. 

Solubility  in  KI+40%  alcohol  at 

Continued. 

25°.— 

Sp.  gr. 

Analysis  of  liquid 
phase 

Analysis  of  solid 
phase  together  with 
adhering  mother 
liquor 

Sp.  gr. 

Analysis  of  liquid 
phase 

Analysis  of  solid 
phase  together  with 
adhering  mother 
liquor 

%  KI 

%i 

%  I 

%   KI 

%  KI             %  I 

%KI 

%i 

(a) 
1.148 
1.191 
1.285 
1.368 
1.427 
1.533 
1.776 
2.250 
2.507 
2.845 

(b 
1.134 
1.530 
1.721 
1.90 
2.11 
2.22 
2.80 
2.99 

(c)Ii 
3.162 

In  equilit 
30.93 
29.87 
28.39 
28.00 
27.60 
27.00 
25.90 
24.90 
24.40 
22.49 
21.50 

)  In  equil 
0.0 
7.36 
10.60 
12.44 
13.74 
15.20 
17.72 
19.30 

ivariant  p 
20.11 
20.03 

20.05 
19.98 
20.08 

20.06 
20.05 

>rium  wit 
0.0 
4.51 
12.48 
18.60 
21.80 
28.00 
40.52 
52.42 
58.93 
65.75 
68.95 

ibrium  wi 
23.04 
43.05 
49.38 
55.33 
59.26 
62.66 
69.10 
71.90 

oint.    Ex 
72.51 
72.46 

72.54 
72.44 
72.51 

72.44 

72.48 

ti  excess 

89.13 
86.60 
87.30 
85.75 
84.39 
81.05 
76.21 
73.20 
71.66 
70.04 

th  excess: 
0.0 
1.40 
2.50 
3.72 
4.41 
5.80 
7.15 
7.45 

cess  KI 
2l!  84 

7^40 
20.61 

33^46 

KI. 
0.0 
0.71 
2.27 
3.21 
4.25 
6.05 
10.30 
16.73 
21.04 
24.15 
26.42 

a. 
i 

88.76 
88.21 
87.10 
86.60 
85.20 
85.49 
88.96 

and  I. 

74.64" 
KI+I 

89!gi'l 
74.09 
KI+I 

33.19KI 

(t 
0.962 
1.292 
1.581 

2'.000 
2.173 
1.749 
2.902 

(c)I 
3.246 

0  In  equilibrium  w 
0.0          2.97 
8.45      28.70 
12.56      40.63 
15.20      49.95 
16.02      52.95 
17.18      57.38 
19.20      66.89 
20.12      69.10 
nvariant  point.    EJ 
22.50      70.79 
22.43      70.88 

ith  excess 
0.0 
1.85 
3.41 
4.98 
5.60 
6.61 
8.45 
7.08 
ccess  KI  i 
19.48 
69.37 

I. 

84.51 
84.02 
83.81 
82.96 
83.60 
85.16 
88.81 
mdl. 
76.24 
26.14 

(Parsons  and  Corliss,  J.  Am.  Chem.  Soc.  1910. 
32.  1372.) 
See  also  under  KI.  . 

-  Sol.      in      KI  +nitrobenzene.       (Dawson, 
Chem.  Soc.  1902,  81.  529.) 
.Solubility  in  KIO3+Aq  is  the  same  as  in 
H2O.    (Lami,  C.  A.  1909.  1622.) 

Solubility  of  I2  in  KBr+Aq  at  25°. 

G. 

KBr  per  1. 

G.  atoms  Iz 

per  1. 

60.6 
106.9 
175.9 
229.8 
281.9 
330.6 
377.1 
411.0 
461.7 
509.8 
548.0 
567.9  sat. 

0.0176 
0.0278 
0.0415 
0.0532 
0.0628 
0.0717 
0.0797 
0.0864 
0.0948 
0.1006 
0.1062 
0.1094 

(Parsons  and  Corliss,  J.  Am.  Chem.  Soc.  1910, 
32.  1370.) 

Solubility  in  KI+40%  alcohol  at  25°. 

Sp.  gr. 

Analysis  of  liquid 
phase 

Analysis  of  solid 
phase  together  with 
adhering  mother 
liquor. 

(Bell  and  Buckley,  J.  Am.  Chem.  Soc.  1912, 
34.  13.) 

Solubility  in  NaBr+Aq  at  25°. 

%  KI 

%  I 

%  KI 

%l. 

G.  NaBr  per  1. 

G.  atoms  It  per  1. 

(a] 

1.339 
1.377 
1.455 
1.532 
1.605 
1.655 
1.847 
2.024 
2.169 
2.558 
2.784 

In  equili 

42.10 
40.83 
38.94 
37.41 
36.25 
35.38 
33.26 
31.71 
30.59 
28.56 
26.95 
24.52 
23.04 

Drium  wi 

0.0 
3.76 
10.09 
15.71 
20.52 
24.44 
33.62 
39.99 
44.76 
55.30 
60.27 
65.93 
69.93 

,h  excess 

89.21 
88.80 
88.19 
87.04 
86.08 
83.61 
82  ..06 
80.80 
75.90 
74.77 
72.98 
72.45 

KI. 

0.0 
0.70 
1.90 
3.02 
4.21 
5.11 
8.41 
10.76 
12.35 
18.63 
20.86 
23.61 
25.04 

96.4 

187.7 
271.8 
357.4 
422.4 
499.1 
569.9 
632.0 
679.7 
750.5 
756.1  sat. 

0.0266 

0.0425 
0.0538 
0.0598 
0.0638 
0.0648 
0.0644 
0.0622 
0.0595 
0.0551 
0.0550 

(Bell  and  Buckley,  J.  Am. 
34.  13.) 

Chem.  Soc.  1912, 

412 


IODINE 


100  cc.  of  a  10%  solution  of  SrBr2  dissolve 
0.270  g.  I2  at  13.50.  (Meyer,  Z.  anorg.  1902, 
30.  114.) 

100  cc.  of  a  10%  solution  of  SrCl2  dissolve 
0.066g.  I2  at  18.5°.  (Meyer.) 

100  cc.  of  a  10%  solution  of  SrI2  dissolve 
6.616g.  I2  at  13.5°.  (Meyer.) 

Solubility  in  salts +Aq  at  25°. 


Salt  +Aq 

Grams 
la  sol.  in 
1  liter 

Salt  +Aq 

Grams 
I2  sol.  in 
1  liter 

i^-N.Na2SO4 
^-N.K2S04 
i^-N.(NH4)2S04 
N.NaNO3 
N.KNO3 
N.NH4NO3 

0.160 
0.238 
0.246 
0.257 
0.266 
0.375 

N.NaCl 
N.KC1 
N.NH4C1 
N.NaBr 
N.KBr 
N.NH4Br 

0.575 
0.658 
0.735 
3.29 
3.801 
4.003 

(McLauchlan,  Z.  phys.  Ch.  1903,  44.  617.) 

1.14  g.  are  sol.  in  100  ccm.  liquid  H2S.  (An- 
tony, Gazz.  ch.  it.  1905,  35,  (1)  206.) 

Sol.  in  liquid  NH3.  (Franklin,  Am.  ch.  J. 
1898,  20.  822.) 

SI.  sol.  in  liquid  CO2.  (Biichner,  Z.  phys. 
Ch.  1906,  54.  674.) 

Sol.  in  liquid  SO2  (Sestini),  and  SO2 
(Weber). 

100  pts.  AsCl3  dissolve  8.42  pts.  I  at  0°; 
11.88  pts.  I  at  15°;  36.89  pts.  I  at  96°. 
(Sloan,  C.  N.  46. 194.) 

Sol.  in  liquid  SO2,  AsCl3,  SO2C12,  and 
acetaldehyde.  (Walden,  Z.  phys.  Ch.  1903, 
43.  407.) 

Very  sol.  in  liquid  NO2.  (Frankland, 
Chem.  Soc.  1901,  79.  1361.) 

Sol.  in  10-12  pts.  alcohol.     (Wittstein.) 

Sol.  in  wood-spirit.     (Playfair.) 

Abundantly  sol.  in  amyl  (Pelletan),  and 
hexyl  alcohol  (Bouis). 

Iodine  is  sol.  in  20  pts.  alcohol,  110  pts.  oil, 
7000  pts.  H2O,  100  pts.  glycerine.  (Cap  and 
Garot,  J.  Pharm.  (3)  26. 80.) 

Solubility  of  I2  in  C2H5OH+Aq  at  room 
temperature  (14.5°— 15.1°). 


Volumes  of  C2H5OH  in 
100  volumes  of  C2H5OH 
+H20 

Ccm.  of   1/10-normal 
iodine  in  5   cc.   of  the 
solution 

100 

61.7 

90 

29.4 

80 

16.6 

70 

9.2 

60 

4.45 

50 

3.4 

40 

1.0 

30 

0.4 

20 

0.25 

10 

0.2 

0 

0.0 

(Bruner,  Z.  phys.  Ch.  1898,  26.  150.) 


Solubility  of  I2  in  C3H7OH+Aq  at  room 
temperature  (14.5°— 15.1°). 


Volumes  of  C3H7OH  in 
100  volumes  of  C3H;OH 
,     +H20 

Ccm.   of   1/10-normal 
iodine  in  5  cc.  of  the 
solution 

100 

58.8 

90 

36.0 

80 

23.6 

70 

16.1 

60 

10.7 

,50 

6.4 

40 

3.7 

30 

1.56 

20 

0.42 

•.       10 

0.19 

0 

.... 

(Bruner,  Z.  phys.  Ch.  1898,  26.  150.) 
Solubility  in  ethyl  alcohol +Aq  at  25°. 


Molecules  of 
C2H5OH  in  100 
molecules 
C2H5OH  +H2O 

Molecule's  of  H2O 
in  100  molecules 
C2H6OH  +H2O 

Normality  of  the 
iodine  solution 

0.0 

100 

0.0022 

0.03 

99.  7(?) 

0.0024 

0.06 

99.  4(?) 

0.0024 

1.12 

98.88 

0.0023 

1.83 

98.27(?) 

0.0025 

9.40 

90.60 

0.0059 

13.48 

86.52 

0.0111 

23.80 

76.20 

0.0617 

50.80 

49.20 

0.4326 

100 

0 

1.590 

(McLauchlan,  Z.  phys.  Ch.  1903,  44.  627.) 
Solubility  in  acetic  acid+Aq  at  25°. 


Molecules  of 
CEbCOOH  in  100 
molecules 
CHsCOOH  +H2O 

Molecules  of  H2O 
in  100  molecules 
CHsCOOH  +H2O 

Normality  of  the 
iodine  solution 

0.0 

6.98 
16.40 
31.90 
55.70 
100 

100 

93.02 
83.60 
68.10 
44.30 
0 

0.0022 
0.0049 
0.0112 
0.0331 

0.0882 
0.205 

(McLauchlan,  Z.  phys.  Ch.  1903,  44.  627.) 

Very  sol.  in  ether,  chloroform,  and  bromo- 
form. 

Solubility  in  ether. 
100  g.  of  the  sat.  solution  contain  at: 
—83°         —90°         —108° 
15.39         14.58         15. 09  g.  I2. 
(Arctowski,  Z.  anorg.  1896,  11.  276.) 

About  as  sol.  in  all  fatty  oils  as  in  CHC13, 
etc.    (Gruel,  Arch.  Pharm.  223.  431.) 


IODINE 


413 


Sol.  in  56.6  pts.  chloroform  at  10°.    (Dun- 
can, Pharm.  J.  Trans.  51.  544.) 
Solubility  in  CHC13. 
100  g.  of  the  sat.  solution  contain  at: 
—49°    —55.5°    —60°    —69.5°   —73.5° 
0.188     0.144     0.129      0.089     O.OSOg.  I2. 
(Arctowski,  Z.  anorg.  1896,  11.  276.) 

Very  sol.  in  methvlene  iodide.     (Retgers, 
Z.  anorg.  3.  343.) 

Solubility  of  I2  in  C6H6+CHC13  at  room 
temperature  (14.5°—  15.1°). 

Solubility  of  I2  in.  CS2+CC14  at  room 
temperature  (14.5°  —  15.1°). 

Volumes  of  CS2  in  100 
volumes  of  CS2  +CCU 

Ccm.  of  1/10-normal  iodine 
in  5  cc.  of  the  solution 

100 
90 
80 
70 
60 
50 
40 
30 
20 
10 
0 

69.1 
56.9 
48.6 
40.7 
33.9 
26.9 
21.8 
17.7 
13.25 
10.2 
8.1 

Volumes  of  C6H6  in  100 
volumes  of  CeHe+CHCU 

Ccm.  of  1/10-normal  iodine 
in  5  cc.  of  the  solution 

100 
90 
80 
70 
60 
50 
40 
30 
20 
10 
0 

41.05 

38.8 
34.6 
30.5 
27.4 
24.4 
21.0        %%- 
19.2          * 
17.8 
16.0 
14.3 

(Bruner.) 

Solubility  of  I2  in  C2H5OH+CHC13  at  room 
temperature  (14.5°—  15.1°). 

Volumes  of  CiHsOH  in 
100  volumes  of  C2H5OH  + 
CHCh 

Ccm.  of  1/10-normal  iodine 
in  5  cc.  of  the  solution 

100 

90 
80 
70 
60 
50 
40 
30 
20 
10 
0 

61.7 
37.1 
34.2 
30.7 
27.9 
26.1 
24.6 
22.7 
19.9 
17.1 
14.25 

(Bruner,  Z.  phys.  Ch.  1898,  26.  147.) 

Solubility  of  I2  in  CS2+CHC13  at  room 
temperature  (14.5°—  15.1°). 

Volumes  of  CS2  in  100 
volumes  of  CS2  +CHCU 

Ccm.  of  1/10-normal  iodine 
in  5  cc.  of  the  solution 

100 
90 
80 
70 
60 
50 
40 
30 
20 
10 
0 

69.4 
62.7 
55.9 
47.9 
42.0 
35.8 
30.4 
25.3 
20.8 
17.0 
14.3 

(Bruner.) 

Solubility  of  I2  in  C3H7OH+CHC13  at  room 
temperature  (14.5°—  15.1°). 

Volumes  of  CsHrOH  in 
100  volumes  of  CzR-.OH 
+CHC13 

Ccm.  of  1/10-normal  iodine 
in  5  cc.  of  the  solution 

(Bruner.) 

Solubility  of  I2  in  C6H6+CC14  at  room 
temperature  (14.5°  —  15.1°). 

100 

90 
80 
70 
60 
50 
40 
30 
20 
10 
0 

58.8 
51.9 
44.2 
35.4 
31.8 
30.8 
27.9 
25.3 
21.8 
17.8 
14.25 

Volumes  of  C6H6  in  100 
volumes  of  CePU+CCU 

Ccm.  of  1/10-normal  iodine 
in  5  cc.  of  the  solution 

100 
90 
80 
70 
60 
50 
40 
30 
20 
10 
0 

41.05 
37.2 
33.6 
29.6 
26.1 
22.4 
19.25 
16.1 
13.4 
10.75 
8.1 

(Bruner.) 

Sol.  in  acetone.     (Naumann,  B.  1904,  37. 
4328);  (Eidmanri,  C.  C.  1999,  II.  1014.) 
Sol.  in  methyl  acetate  (Naumann,  B.  1909, 
42.    3790);    ethyl    acetate.      (Naumann,    B. 
1904,  37.  3601.) 
Sol.  in  allyl  mustard  oil,  phenyl  mustard 

(Bruner.) 

414 


IODINE 


oil,  phenyl  isocyanate,  pyridine,  and  alcohol. 
(Mathews,  J.  phys.  Chem.  1905,  9.  649.) 

Solubility  of  I2  in  glycerine +Aq  at  25°. 
G  =  g.  glycerine  in  100  g.  glycerine +Aq. 
I2  =  g.  la  in  100  cc.  of  the  solution. 


G 

I2 

Sp.  gr. 

0 

0.0304 

0.9979 

7.15 

0.0342 

1.0198 

20.44 

0.0482 

1.0471 

31.55 

0.0621 

1.0750 

40.95 

0.0875 

1.0995 

48.7 

0.135 

1  .  1207 

69.2 

0.278 

1  .  1765 

100 

1.223 

1.2646 

(Herz  and  Knoch,  Z.  anorg.  1905,  45.  269.) 

1   1.   N-NH4C2H3O2+Aq   dissolves  0.440 
g.  I2  at  25°. 

1  1.  0.7  N-(NH4)2C2O4+Aq  dissolves  0.980 
g.  I2  at  25°. 

(McLauchlan,  Z.  phys.  Ch.  1903,  44.  617.) 

Very  sol.  in  benzonitrile.     (Naumann,  B. 
1914,  47.  1369.) 


1  1.  CC14  dissolves  30.33  g.  I2  at  25°. 
(Jakowkin,  Z.  phys.  Ch.  1895,  18.  590.) 

Solubility  in  CS2. 

100  g.  of  the  sat.  solution  contain  at: 
—80°         —87°         —92.5°         —94° 
0.509         0.440         0.391  0.378g. 

(Arctowski,  Z.  anorg.  1896,  11.  274.) 


When  an  aqueous  solution  of  I  is  shaken 
with  CS2,  400  pts.  go  into  solution  in  CS2  for  1 
pt.  remaining  in  H2O.  (Berthelot  and  Jung- 
fleisch,  C.  R.  69.  338.) 

Abundantly  sol.  in  methane.  (Villard, 
A.  ch.  1897,  (7)  10.  387.) 

Easily  sol.  in  hot,  less  in  cold  naphtha. 
(Pelletier  and  Walker.) 

Sol.  in  about  8  pts.  hot  petroleum  from 
Amiano.  (de  Saussure.) 

SI.  sol.  in  cold,  more  readily  in  hot  ben- 
zene. (Mansfield.)  Easily  sol.  in  benzene. 
(Moride,  A.  ch.  (3)  39.  452.) 

Solubility  in  benzene. 

100  g.  of  the  sat.  solution  contain  at: 
4.7°          6.6°      10.5°      13.7°      16.3° 
8.08         8.63     9.60       10.44     11.23g.  12. 
(Arctowski,  Z.  anorg.  1896,  11.  276.) 

1 1.  benzene  sat.  with  iodine  at  25°  contains 
139  g- iodine.  Abegg,  Z.  anorg.  1906,  50. 
409.) 

1  1.  nitrobenzene  dissolves  50.62  g.  I2  at 
16-17°.  (Dawson  and  Gawler,  Chem.  Soc. 
1902,  81.  524.) 


oomDinty  in  i^s2  at  i  . 

Solubility  of  I2  in  nitrobenzene  +  iodides  at 

t 

Grams  iodine  in  100  g.  of  sat. 

room  temp. 

solution 

G.  per  1. 

0.32 

Salt 

—  100 

- 

—  95 

0.37 

Salt 

12 

—  90 

0.41 

KI 

12.35 

112.7 

—  85 

0.46 

45.56 

295.7 

—  80 

0.51 

115.8 

698.2 

—  75 

0.55 

155.2 

943.6 

—  25 

3.47 

Nal 

13.55 

57.7 

125 
393 

—  20 

4.14 

109.1 

738 

—  15 

4.82 

228. 

1251 

—  10 

5.52 

Rbl 

85.4 

421 

—    5 

6.58 

a 

217.5 

1060 

0 

7.89 

Lil 

84.1 

642 

,-f     5 
10 
15 
20 
25 
30 
36 
40 
42 

9.21 
10.51 
12.35 
14.62 
16.92 
19.26 
22.67 
25.22 
26.75 

Csl 

« 

NH4I 

a 

SrI2 

BaI2 

« 

Aniline  hydriodide 
Dimethyl  aniline  hydriodide 

48.2 
223. 
69.5 
94.3 
106.5 
42.2 
158.5 
164 
160 

213 

858 
482 
669 
599 
237 
809 
721 
626 

(Arctowski,  Z.  anorg.  1894,  6.  404.) 

Tetramethylammonium 
iodide 

49.3 

266 

1  1.  CS2  dissolves  230  g.  I2  at  25°. 

1    1     r.TTRr.  rlifianliroa   1  »Q  fifi   o-     !„   a  <-   9*° 

tt 

51.4 

280 

(Dawson  and  Goodson,  Chem.  Soc.  1904,  85. 
796.) 

Sol  in  quinoline.  (Beckmann  and  Gabel, 
Z.  anorg.  1906,  51.  236.)  . 

Easily  sol.  in  oil  of  turpentine,  but  an  explo- 
sion soon  occurs.  (Walker.) 

Sol.  in  oil  of  mandarin.    (Luca.) 


IODINE 


415 


Sol.  in  oil  of  arnica  root.    (Zeller.) 

Very  sol.  in  CS2,  lignone,  furfurol,  glycerine, 
aldehyde,  chloral,  warm  retinole,  toluene,  sali- 
cylic acid,  methyl  nitrate,  methyl  salicylate, 
mercaptan,  amyl  carbamate,  ethyl  sulp hyd- 
rate, allyl  iodide,  ethyl  disulphocarbonate, 
carbon  chloride,  SC12,  IC13,  H2S5,  chloro- 
chromic  acid,  amyl  valerianate,  valerianic 
acid,  warm  butyric  acid,  creosote,  aniline, 
quinoline,  methylsalicylic  acid.  Quickly  sol. 
in  oil  of  dill,  peppermint,  sassafras,  and  tansy. 
Slowly  sol.  in  oil  of  cloves,  cinnamon,  cajeput, 
and  rue.  Other  essential  oils  decompose  it. 
(Various  authorities.) 

Sol.  in  potassium  croconate + Aq.  (Gmelin.) 

Sol.  in  potassium  antimony  tartrate+Aq. 
176  pts.  H2O-f6  pts.  potassium  antimony 
tartrate  dissolve  2.75  pts.  I;  378  pts.  H26 
+6  pts.  potassium  antimony  tartrate  dissolve 
4.12  pts.  I. 

More  sol.  in  tannic  acid  than  in  H2O.  1  pt. 
I  is  sol.  in  450  pts.  H2O  with  3.3  pts.  tannic 
acid  at  12°;  1  pt.  I  is  sol.  in  240  pts.  H2O  with 
0.015  pt.  tannic  acid  at  about  30°.  (Roller, 
Zeit.  Ch.  1866.  380.) 

200  g.  H2O  containing  0.3-g.  tannic  acid 
dissolve  1.0  g.  I.  (Hager,  Comm.  1883.) 

Sol.  in  considerable  quantity,  especially  on 
warming,  in  resorcin,  orcin,  or  phloroglu- 
cin-f-Aq,  without  coloration  or  formation  of 
HI-j-Aq.  These  solutions  withdraw  1  from 
CS2  solution,  and  do  not  give  it  up  on  boiling, 
but  on  evaporation  in  vacuo  the  I  is  sublimed 
in  a  pure  state.  (Hlasiwetz,  Z.  anal.  6.  447.) 

Partition  coefficient  for  iodine  between  CS2 
arid  Aq  at  25°C. 

A  =  concentration  of  the  water  layer. 

C  =  concentration  of  the  carbon  bisulphide 
layer. 


A 

C 

h=C/A 

0.2913 
0.1934 
0.1276 
0.0818 
0.0516 

25.61 
16.54 
10.88 
6.966 
4.412 

87.91 
85.51 
85.30 
85.13 

85.77 

(Jakowkin,  Z.  phys.  Ch.  1895, 

18.  586-588.) 

G.  alcohol  in  100  cc.  of 
mixture 

C  aq.  alcohol 

ccs2        *  10 

30.5 
26.7 
22.9 
19.1 
16.3 
11.4 
7.6 

1.29 
0.76 
0.49 
0.34 
0.28 
0.23 
0.20 

A 

C 

h=C/A 

0.2571 

167.6 

651.8 

0.2195 

140.2 

638.7 

0.1947 

122.0 

626.4 

0.1743 

108.3 

620.0 

0.1605 

98.27 

612.2 

0.1229 

73.23 

595.8 

0.1104 

65.81 

596.0 

0.0939 

55.29 

590.5 

0.0518 

30.36 

586.2 

Partition  coefficient  for  iodine  between  CHBrj 

and  Aq  at  25°C. 

A  =  concentration  of  the  water  layer. 
C  =  concentration  of  the  CHBr3  layer. 


Partition  coefficient  for  iodine  between  CC14 

and  Aq  at  25°C. 

A  =  concentration  of  the  water  layer. 
C  =  concentration  of  the  CC14  layer. 


(Osaka,  Chem.  Soc.  1905,  88.  (2)  811.) 


Division  of  iodine  between  CS2  and 

Na2SO4+Aqat25°. 
A  =  concentration  of  I  in  H2O  layer. 
C  =  concentration  of  I  in  CS2  layer. 


Na2SOi  +Aq 

A 

C 

1-N 

1/2-N 
Vr-N 

Va-N 

0.1518 
0.1809 
0.2022 
0.2138 

142.4 
141.7 
143.6 
142.4 

Division  of  iodine  between  CS2  and  NaNOs 
+Aq. 

NaNOs  +Aq 

A 

C 

1-N 
Vr-N' 
Vr-N 

0.1923 
0.2090 
0.2164 

142.4 
143.7 
143.5 

(Jakowkin,  Z.  phys.  Ch.  1896,  20.  25.) 

Partition  between  CHC13  and  glycerine. 
C=millimols  iodine  in  10  g.  CHC13  layer. 
W  =  millimols   iodine   in    10   g.    glycerine 
layer. 


A 

C 

g=C/A 

C 

w 

c/w 

0.2736 
0.1752 
0.1084 
0.0757 

144.36 
85.11 
49.93 
32.65 

527.6 

485.7 
460.5 
431.7 

0.564 
0.919 
0.151 

0.244 
0.397 
0.500 

2.31 
2.32 
2.30 

0.0517 

22.19 

429.3 

(Herz,  Z.  Elektrochem.  1910,  16.  870.) 

416 


IODINE  BROMIDE 


Partition  of  I2  between  CHC13  and  other 
solvents. 

C  =millimols  iodine  in  10  ccm.  of  the  CHC13 
layer. 

W  =  millimols  iodine  in  10  ccm.  of  the  other 
layer. 


Distribution  of  I2  between  glycerine  and  CC14 
att°. 

MI  =  concentration  of  I2  in  CC14  layer  ex- 
pressed in  g.-mol.  per  1. 

M2  =  concentration  of  I2  in  glycerine  layer 
expressed  in  g.-mol.  per  1, 


Other  Solvent 

C 

w 

c/w 

t° 

Mi 

Mi 

Water 

0.338 
1.546 
2.318 
3.207 
3.439 

0.0025 
0.0120 
0.0184 
0.0242 
0.0259 

134.6 
129.0 
126.3 
132.8 
132.8 

25° 

0.002230 
0.0024113 
0.0048227 
0.010452 
0.038973 
0.04598 
0.05820 

0.0014386 
0.0014595 
0.0027014 
0.005581 
0.019959 
0.023948 
0.030097 

75%  by  vol.  H2O  + 
25%  by  vol.  glycerine 

1.217 
1.893 
2.434 
3.219 

0.0183 
0.0290 
0.0367 
0.0483 

66.32 
65.33 
66.31 
66.65 

40° 

0.00227 
0.00239 
0.00461 
0.01092 
0.02540 
0.04091 
0.06074 

0.00127 
0.00138 
0.00272 
0.00482 
0.01116 
0.01749 
0.02701 

50%  by  vol.  H2O  + 
•50%  by  vol.  glycerine 

1.217 
1.835 
2.376 
3.294 

0.0405 
0.0609 
0.0782 
0.1020 

30.0 
30.1 
30.4 
32.2 

25%  by  vol.  H2O  + 
75%  by  vol.  glycerine 

1.188 
1.806 
2.656 
2.859 
3.400 

0.116 
0.173 
0.249 
0.265 
0.312 

10.25 
10.45 
10.66 
10.80 
10.93 

50° 

0.00257 
0.00500 
0.01363 
0.02549 
0.04167 
0.06309 

0.00118 
0.00225 
0.00596 
0.01050 
0.01693 
0.02502 

(Herz,  Z.  Elektrochem.  1910,  16.  870.) 

Distribution    of    I2    between    benzene    and 
glycerine  at  t°. 
MI  =  concentration  of  I2  in  benzene  layer 
expressed  in  g.-mol.  per  1. 
M2  =  concentration  of  I2  in  glycerine  layer 
expressed  in  g.-mol.  per  1. 

(Landau,  Z.  phys.  Ch.  1910,  73.  203.) 

Distribution  of  I2  between  ether  and  ethylene 
glycol  at  t°. 
MI  =  concentration   of  I2  in   ether  layer, 
expressed  in  g.-mol.  per  1. 
M2  =  concentration  of  I2  in  C2H6O2  layer, 
expressed  in  g.-mol.  per  1. 

t° 

Mi 

Ms 

25° 

0.00757 
0.01610 
0.02719 
0.04024 
0.06255 
0.07923 
0.10243 
0.12201 
0.13342 
0.16734 

0.001604 
0.002664 
0.004115 
0.005794 
O.OOS34 
0.01033 
0.01324 
0.01559 
0.01668 
0.02081 

t° 

Mi 

M2 

0° 

0.00843 
0.03082 
0.06551 
0.08105 
0.12528 
0.31511 

0.00571 
0.01713 
0.03736 
0.04605 
0.07148 
0.17524 

40° 

0.008545 
0.01544 
0.04432 
0.095004 
0.13271 
0.18508 

0.00181 
0.002593 
0.006242 
0.012013 
0.01632 
0.02193 

25° 

0.00870 
0.01677 
0.02710 
0.03046 
0.06385 
0.11951 
0.30820 

0.00571 
0.01001 
0.01586 
0.01713 
0.03594 
0.06725 
0.17524 

50° 

0.00865 
0.01523 
0.02683 
0.04413 
0.0620 
0.07832 
0.10153 
0.12166 
0.13199 
0.18438 

0.00184 
0.00253 
0.00390 
0.00576 
0.00744 
0.00942 
0.01214 
0.0145 
0.01560 
0.02122 

(Landau,  Z.  phys.  Ch.  1910,  73.  205.) 

Iodine  mowobromide,  IBr. 
Slowly  sol.  in  H2O  with  slight  decomp. 
Sol.  in  CHC13,  CS2,  ether,  and  alcohol. 
+5H2O.     (Lowig,  Pogg.  14.  485.)     Does 
not  exist.    (Bornemann,  A.  189.  183.) 

(Landau,  Z.  phys.  Ch.  1910,  73.  202.) 

IODINE  SULPHIDE 


417 


Iodine  pew/abromide,  IBr5(?). 

Sol.  iri  H2O  with  separation  of  iodine. 
(Lowig,  Pogg.  14.  485.) 

Iodine  wonochloride,  IC1. 

Decomp.  by  H2O;  sol.  without  decomp.  in 
alcohol,  ether,  and  HCl+Aq. 

Sol.  in  CS2. 

Iodine  hydrogen  chloride,  IC1,  HC1. 

Unstable.  Sol.  in  ether.  (Schiitzenberger, 
C.  R.  84.  389.) 

Iodine  ^nchloride,  IC13. 

Deliquescent.  With  H2O,  a  part  is  dissolved 
without  decpmp.,  and  the  rest  is  decomp. 
The  aqueous  solution  contains  more  un- 
changed Ids,  the  more  cone,  it  is.  (Serullas.) 
Precipitated  from  aqueous  solution  by  H2SO4. 
Sol.  in  HCl+Aq.  Sol.  in  warm  cone.  H2SO4 
without  decomp.  Sol.  in  alcohol,  and  ben- 
zene. Decomp.  by  small  amount  of  CS2. 
(Christomanos,  B.  10.  434.)  Ether  does  not 
remove  it  from  aqueous  solution.  (Serullas.) 

Iodine  lithium  chloride,  IC13,  LiCl+4H2O. 
See  Lithium  chloroiodide. 

Iodine  trichloride  magnesium  chloride,  2IC13, 
MgCl2+5H2O. 

Very  deliquescent  and  easily  decomposed. 
(Filhol,  J.  Pharm.  25.  442.) 

+8H2O.  Hydroscopic.  (Weinland,  Z. 
anorg.  1902,  30.  141.) 

Iodine  ^'chloride  manganous  chloride,  2IC13, 

MnCl2+8H2O. 

Hydroscopic.  (Weinland,  Z.  anorg.  1902, 
30.  139.). 

Iodine    bichloride    nickel    chloride,    2IC13, 

MC12+8H2O. 

Hydroscopic.  CC14  dissolves  out  IC13. 
(Weinland,  Z.  anorg.  1902,  30.  138.) 

Iodine  raonochloride  phosphorus  pentathloT- 

ide,  IC1,  PC15. 
Very  deliquescent;  decomp.  by  H2O. 

Iodine  potassium  chloride,  IC13,  KC1. 

Sol.  in  H2O  with  decomp. 

Ether  dissolves  out  IC13.  (Filhol,  J.  Pharm. 
25.  433,  506.) 

See  Potassium  chloroiodide. 

Iodine  sodium  chloride,  IC13,  NaCl+2H2O. 
See  Sodium  chloroiodide. 

Iodine  trichloride  strontium  chloride,  2IC13, 

SrCl2+8H2O. 

Hydroscopic.  (Weinland,  Z.  anorg.  1902. 
30.  142.) 


Iodine  trichloride  sulphur  te^rachloride,  IC13, 

SC14. 

Very  deliquescent  in  air;  decomp.  by  H2O. 
Decomp.  with  formation  of  clear  solution  by 
dil.  HNO3+Aq.    (Weber,  Pogg.  128.  459.) 
SC12,  2IC13.    (Jaillard,  J.  B.  1860.  95.) 
Correct  formula  is  as  above.    (Weber,  I.  c.) 
2IC1,,  SC14.    Sol.  in  S02C12,  SOC1,,  POC13, 
warm  SC12,  petroleum  ether,  ligroin,  CHCls, 
CC14,  CS2  and  abs.  ether.    (Ruff,  B.  1904,  37. 
4519.) 

Iodine  trichloride  zinc  chloride,  2IC13,  ZnCl2+ 

8H2O. 

Unstable.  Hydroscopic.  (Weinland,  Z. 
ahorg.  1902,  30.  140.) 

Iodine  perctafluoride,  IF5. 

Fumes  in  air;  decomp.  with  H2O.  (Gore. 
C.  N.  24.  291.) 

Decomp.  by  H20  into  iodic  acid  and  HF. 
Decomp.  by  solutions  of  the  alkalies.  (Mois- 
san,  C.  R.  1902,  135.  564.) 

Iodine  ^n'oxide,  I2O3. 

Decomp.  by  H2O.  (Ogier,  C.  R.  85.  957; 
86.  722.) 

Probably  a  mixture. 

Iodine  tafroxide,  I2O4(?). 

Insol.  in  cold,  decomp.  by  hot  H2O;  insol. 
in  alcohol.  Decomp.  by  HNO3+Aq.  Sol.  in 
H2SO4.  (Millon,  J.  pr.  34.  319,  337.) 

Iodine  pentoxide,  I2O5. 

Very  sol.  in  H2O,  and  in  dil.  alcohol. 
Insol.  in  absolute  alcohol,  ether,  CS2,  chloro- 
form, and  hydrocarbons. 

Forms  hydrates,  iodic  acid  HIO3,  and 
3I2O5,  H2O;  insol.  in  ordinary  alcohol. 

For  sp.  gr.  of  aqueous  solution,  see  iodic 
acid. 

Iodine  oxides,  IioO19,  I3Oi3. 

The  compounds,  IioOig  (Millon,  J.  pr.  34. 
336),  and  I3O13  (Kammerer,  J.  pr.  83.  81), 
are  probably  mixtures. 

Millon's  oxides  are  impure  I2O4.  (Kap- 
peler,  B.  1911,  44.  3496.) 

Iodine  sulphur  oxide,  5I2O5,  SO3. 
Decomp.  by  H2O.    (Kammerer.) 
I2OS,  3SO3.    Decomp.  by  H2O;  si.  sol.  in 

hot  SO4.    (Weber,  B.  20.  86.) 

=  (IO)2(SO4)3.    lodyl  sulphate  (?). 

Iodine  oxyfluoride,  IOF3+5H2O. 

Fumes  in  the  air.  (Weinland,  Z.  anorg. 
1908,  60.  163.) 

Iodine  sulphide,  S2I2. 

Sol.  in  CS2.  (Linebarger,  Am.  Ch.  J.  1895. 
17.  57.) 


418 


IODINE  SULPHOXIDE 


Iodine  sulphoxide,  I2SO8(?). 

Decomp.  by  H2O.    (Schultz-Sellack.) 
I2(SO3)2(?).    Decomp.  by  H2O.    (Weber,  J. 

pr.  (2)  26.  224.) 

Is(SO8)«(?).    As  above.    (Weber.) 
See  also  lodosulphuric  anhydride. 

lodiridic  acid. 

Ammonium  iodiridate,  (NH4)2IrI6. 

Very  easily  sol.  in  cold  H2O,  decomp.  on 
warming.  Insol.  in  alcohol.  (Oppler,  J.  B. 
1857.  263.) 

Potassium  iodiridate,  K2IrI6. 
Very  easily  sol.  in  H2O.    Insol.  in  alcohol. 

Sodium  iodiridate,  Na2IrI6. 

Insol.  in  cold.  si.  sol.  in  hot  H2O.  Easily 
sol.  in  acids.  (Oppler.) 

lodiridous  acid. 

Ammonium  iodiridite,  (NH4)6lr2Ii2+H2O. 

Very  sol.  in  H20,  but  decomp.  on  warming. 
(Oppler.) 

Potassium  iodiridite,  K6Ir2Ii2. 

Insol.  in  H2O,  or  alcohol.  Slowly  sol.  in 
acids;  easily  in  warm  alkalies  +Aq. 

Silver  iodiridite,  Ag6Ir2Ii2. 
Ppt. 

lodochloroplatiml/amine  chloride, 

(?1Pt(N2H6Cl)2. 
81.  sol.  in  H2O. 

lodochromic  acid. 

Potassium  iodochromate,  KCr03I. 

Decomp.  by  boiling  H2O.    (Guyot,  C.  R. 
73.  46.) 
.  See  also  Chromoiodic  acid. 

lodomolybdic  acid. 
See  Molybdoiodic  acid. 

lodonitratoplatinraonodiamine  bromide, 

I    pf(NH3)2Brm 
NO3rtNH3Br     u;> 
Very  si.  sol.  in  H2O.    (Cleve.) 

lodonitritoplatin^'amine  nitrate, 

I(N02)Pt(N2H6)2(N03)2. 
Quite  easily  sol.  in  hot  H2O.    (Cleve.) 

lodopalladous  acid. 

Potassium  iodopalladite. 
Deliquescent.    (Lassaigne.) 


lodophosphoric  acid. 
See  Phosphoiodic  acid. 

lodoplatinamine  iodide,  I2Pt(NH3I)2. 

Sol.  in  H2O,  especially  easily  if  boiling. 
(Cleve.) 

lodoplatin^amine  iodide,  I2Pt(N2IU)2. 
Sol.  in  H20,  especially  when  hot.    (Cleve.) 

mercuric  iodide,  I2Pt(N2H6I)2,  2HgI2. 

Extremely  difficultly  sol.  in  cold  H2O; 
partly  decomp.  by  boiling.  (Jorgensen,  Gm. 
K.  3.  1214.) 

nitrate,  I2Pt(N2H6NO3)2. 

More  sol.  in  hot  than  cold  H2Q. 

sulphate,  I2Pt(N2H6)2SO4. 

Very  si.  sol.  in  H2O.  (Jorgensen.  J.  pr.  (2) 
15.  429.) 

lodoplatinsew^amine  iodide, 

I3Pt(NH3)2I(?). 

81.  sol.  in  H2O.  (Jorgensen,  J.  pr.  (2)  16. 
345.) 

periodide,  I3Pt(NH3)2I,  I2. 

Moderately  si.  sol.  in  H2O.    (Cleve.) 

lododi'platinamine  iodide,  I2Pt2(N2H6)2I4. 
Insol.  in  H2O. 

lododiplatincfo'amine  anhydroiodide, 

I2Pt2(N2H6)4OI2. 
Insol.  in  NH4OH+Aq. 

—  anhydronitrate,  I2Pt2(N2H6)4O(NO3)2. 
Easily  sol.  in  warm  H2SO3+Aq.    (Cleve.) 

—  iodide,  I2Pt2(N2H6)4I4. 
Ppt. 

—  nitrate,  I2Pt2(N2H6)4(NO3)4+4H2O. 
81.  sol.  in  cold,  moderately  sol.  in  hot  H2O. 

(Cleve.) 

—  phosphate,  I2Pt2(N2H6)4[O3P(OH)]2. 
Nearly  insol.  in  H2O. 


sulphate,  I2Pt2(N2H6)4(S04)2. 


Nearly  insol.  in  H2O. 

—  platoeframine  sulphate,  I2Pt2(N2H6)4SO4, 

Pt(NH3)2S04. 

Very  si.  sol.  in  H2O.  (Carlgren  Sv.  V.  A.  F. 
47.  306.) 

lodoplatinic  acid,  H2PtIe+9H2O. 

Deliquescent.  Easily  sol.  in  H2O,  with  de- 
comp. into  PtI4  and  HI  on  standing  or  warni- 
ng. (Topsoe.) 


IODOSELENATE,  POTASSIUM 


419 


Ammonium  iodoplatinate,  (NH4)2Ptl6. 

Easily  sol.  in  H2O.    (Topsoe.) 

NHJ,   PtI4.     SI.   sol.   in   H2O;   insol.   in 
alcohol.    (Lassaigne,  A.  ch.  (2)  51.  128.) 

Barium  iodoplatinate,  BaPtle. 

Deliquescent,   but   less   so   than    Na2PtI6 
which  it  otherwise  resembles.    (Lassaigne.) 

Calcium  iodoplatinate,  CaPtI6  +  12H2O. 

Not  so  deliquescent  as  Na  salt. 

Cobalt  iodoplatinate,  CoPtI6+9H2O. 
Very  deliquescent. 

Lead  tefraiodoplatinate,  [PtI4(OH)2]Pb, 

Pb(OH)2. 
Ppt.    (Belluci,  C.  C.  1902,  I.  625.) 

Magnesium  iodoplatinate,  MgPtIe+9H2O. 
Sol.  in  H2O. 

Manganese  iodoplatinate,  MnPtI6+9H2O. 
Very  deliquescent. 

Mercuric  ^raiodoplatinate,  [PtI4(OH)2]Hg. 
Ppt.    (Belluci,  C.  C.  1902,  I.  625.) 

Nickel  iodoplatinate,  NiPtI6+9H2O. 
Very  deliquescent. 

Potassium  iodoplatinate,  K2PtI6. 

Easily  sol.  in  H2O.    Insol.  in  alcohol.    Not 
attacked  by  cold  cone.  H2SO4.  * 

Silver  tefraiodoplatinate,  Pt[I4(OH)2]Ag2. 
Ppt.    (Belluci,  C.  C.  1902,  I.  625.) 

Sodium  iodoplatinate,  Na2PtI6+6H2O. 
Not  deliquescent,  but  easily  sol.  in  H2O 


iqi] 
.ol. 


and    alcohol.      (Vauquelin.)      Deliquescent. 

(Lassaigne.) 

Thallium  te(miodoplatinate,  [PtI4(OH)2]Tl2. 
Ppt.    (Belluci,  C.  C.  1902,  I.  625.) 

Zinc  iodoplatinate,  ZnPtI6+9H2O. 
Easily  sol.  in  H2O. 

lodoplatinocyanhydric  acid,  H2Pt(CN)4l2. 
See  Periodoplatinocyanhydric  acid. 

Silver  iodoplatinocyanide,  Ag2(PtI2(CN4)2. 
Ppt.    (Miolati,  Gazz.  ch.  it.  1900,  30.  588.) 

Strontium  iodoplatinocyanide  platinocyanide, 

SrPt(CN)4I2,  10SrPt(CN)4+zH2O. 
(Hoist.) 


lodopurpureochroiaium  chloride, 

ICr(NH3)5Cl2. 

Quite  sol.  in  H2O.  (Jorgensen,  J.  pr.  (2) 
25.  83.) 

chloroplatinate,  ICr(NH3)5PtCl«. 

Precipitate.    (Jorgensen,  I.  c.) 

iodide,  ICr(NH3)6I2. 

Difficultly  sol.  in  H2O.  Insol.  in  HI,  or 
KI+Aq;  insol.  in  alcohol.  (Jorgensen,  1.  c.) 

—  nitrate,  ICr(NH3)5(NO3)2. 
Much  less  sol.  in  H2O  than  the  chloride. 
(Jorgensen,  1.  c.) 

lodopurpureocobaltic  iodide,  CoI(NH3)6I2. 

(Claudet.) 

Does  not  exist.  (Jorgensen,  J.  pr.  (2)  26. 
94.) 

lodopurpureorhodium  chloride, 

IRh(NH3)5Cl2. 

Relatively  easily  sol.  in  H2O;  insol.  in  HC1 
+Aq  and  alcohol.  Insol.  in  KI+Aq.  (Jor- 
gensen, J.  pr.  (2)  27.  433.) 

fluosilicate,  IRh(NH3)5SiF6. 

Nearly  insol.  in  cold  H2O. 

iodoplatinate,  IRh(NH3)5PtI6. 

Ppt. 

iodide,  IRh(NH3)5I2. 

Very  si.  sol.  in  cold  H2O;  more  sol.  in  hot 
H2O;  insol.  in  dil.  HI-f-Aq,  and  alcohol. 
(Jorgensen,  J.  pr.  (2)  27.  433.) 

nitrate,  IRh(NH3)5(NO3)2. 

SI.  sol.  in  H2O,  more  easily  sol.  in  hot  H2O; 
insol.  in  dil.  HNO3+Aq,  and  alcohol. 

sulphate,  IRh(NH3)5SO4,  and  -f  3H2O. 

SI.  sol.  in  even  hot  H2O.    (Jorgensen.) 

lodoselenic  acid. 

Ammonium  iodoselenate,  2(NH4)2O,  I2O5 
2SeO3+H2O. 

Decomp.  by  H2O.  (Weinland,  B.  1903,  36. 
1400.) 

2(NH4)2O,  3I2O5,  2SeO3+5H2O.  Sol.  in 
H2O  with  decomp.(?).  (Weinland.) 

Potassium  iodoselenate,  2K2O,  I2O5,  2SeO3  + 

H2O. 

Decomp.  by  H2O.    (Weinland.) 
2K2O,  3I2O5,  2SeO3+5H2O.    Sol.  in  H2O 

with  decomp.(?)    (Weinland.) 


420 


IODOSELENATE,  RUBIDIUM 


Rubidium  iodoselenate,  2Rb2O,  3I2O5,  2Se03 

+5H20. 
Sol.  inH2O.    (Weinland.) 

lodostannous  acid. 

Data  concerning  solubility  of  SnI2  in  HI  + 
Aq  indicate  formation  of  this  compound. 
(Young,  J.  Am.  Chem.  Soc.  1897,  19.  853.) 

lodosulphobismuthous  acid. 

Cuprous  iodosulphobismuthite,  2Cu2S,  Bi2S3, 

2BiSI. 

Decpmp.  by  H2O  at  ord.  temp.  Decomp. 
by  mineral  acids  with  evolution  of  H2S. 
(Ducatte,  C.  R.  1902,  134.  1213.) 

Lead  iodosulphobismuthite,  PbS,  Bi2S3, 2BiSI. 
Insol.  in  H2O.    Partially  decomp.  by  boil- 
ing H2O.    Decomp.  by  dil.  mineral  acids  with 
evolution  of  H2S.    (Ducatte.) 

*  • 

Io  do  sulphuric  acid. 

Ammonium  iodosulphate,  (NH4)2SO3I2(?). 

Very  sol.  in  H2O.  (Zinno,  N.  Rep.  Pharm. 
20.  449.) 

Mercuric  iodosulphate,  Hg2(SO4)I2. 
See  Mercuric  sulphate  iodide. 

Potassium  iodosulphate,  K2SO3I2(?). 

Sol.  in  7.14  pts.  H2O  at  15°.  (Zinno,  N. 
Rep.  Pharm.  20.  449.) 

Sodium  iodosulphate,  Na2SO3Ia+10H2O. 

Sol.  in  3.64  pts.  H20  at  15°  and  in  dil. 
alcohol.  (Zinno,  N.  Rep.  Pharm.  20.  449.) 

Does  not  exist.  (Michaelis  and  Koethe,  B. 
6.  999.) 

lodosulphuric  anhydride,  ISO3. 

Decomp.  very  violently  by  H2O.  (Weber, 
J.  pr.  (2)  25.  224.) 

Diiodosulphuric  anhydride,  I2SO3. 

Decomp.  with  H2O,  but  not  so  violently  as 
ISO3.  (Weber,  J.  pr.  (2)  25.  224.) 

lodo^n'sulphuric  anhydride,  I(SO3)3. 

Decomp.  by  H2O.    (Weber,  J.  pr.  (2)  25. 

224.) 

lodotelluric  acid. 

Ammonium    iodotellurate,    (NH4)2O,  •  I2Ofi 
2TeO3+6H2O. 

Sol.  in  H2O.  (Weinland,  Z.  anorg.  1901 
28.  52.) 

(NH4)2O,  I2O5,  2TeO3+8H2O.  Sol.  in 
H2O.  (Weinland,  B.  1900,  33.  1017.) 


Caesium  iodotellurate,  Cs2TeI4. 

Insol.  in  Csl,  or  HI+Aq.  Decomp.  slowly 
by  cold,  rapidly  by  hot  H2O.  (Wheeler,  Sill. 
Am.  J.  145.  267.) 

Potassium  iodotellurate,  K2TeI6+2H2O. 

SI.  efflorescent.  Somewhat  sol.  in  KI+Aq, 
and  dil.  HI+Aq.  (Wheeler.) 

K2O,  I2O5,  TeO3+3H2O.  Sol.  in  H2O. 
Partially  decomp.  on  recryst.  from  H2O. 
(Weinland,  Z.  anorg.  1901,  28.  53.) 

K2O,  I2O5,  2TeO3+6H2O.  Sol.  in  H2O 
without  decomp.  (Weinland.) 

Rubidium  iodotellurate,  Rb2TeI6. 

SI.  sol.  in  HI,  or  Rbl+Aq.    Decomp.  by 


H2O.    Somewhat  sol.  in  alco 


q. 
hol. 


(Wheeler.) 


Rb2O,  I2O5,  2TeO3+6H2O.     Sol.  in  H2O. 
(Weinland.) 

lodotetramine  chromium  iodide, 

ICr(NH3)4I2+H20. 
Sol.  in  H2O.    Pptd.  by  alcohol.    (Cleve.) 

lodotetramine  cobaltic  sulphate, 

ICo(NH3)4SO4. 
(Vortmann  and  Blasberg,  B.  22.  2652.) 

lodotungstic  acid. 
See  Tungstoiodic  acid. 

lodous  acid,  I2O3. 
See  Iodine  ^noxide. 

lodovanadic  acid,  I2O5,  V2O5+5H2O. 

Very  easily  sol.  in  H2O. 

2V2O5,  3I2O5+18H2O.    (Ditte,  C.  R.  102. 
757.) 

Ammonium  iodovanadate,  3(NH4)2O,  2V2O5, 

5I2O6+20H2O. 
Sol.  in  H2O.    (Ditte,  C.  R.  102.  1019.) 

Irididiamine  compounds,  Cl2Ir(NH3)4X2. 
See  Chloriridfamine  compounds'. 

Iridic  acid. 


Potassium  iridate  (?). 

Sol.  in  H2O  and  HCl-f  Aq. 


Iridicyanhydric  acid,  H3Ir(CN)6. 

Easily  sol.  in  H2O,  still  more  easily  in  al- 
cohol, less  in  ether.    (Martius,  A.  117.  369.) 

Barium  iridicyanide,  Ba3fIr(CN)6]2+18H2O. 
Efflorescent.    Easily  sol.  in  hot  or  cold  H2O. 
Nearly  insol.  in  alcohol.     Not  decomp.  by 
acids. 


IRIDIUM  PHOSPHORUS  SULPHUR  CHLORIDE 


421 


Cupric  iridicyanide  ammonia,  Cu3Ir9(CN)i2, 

6NH3+4H2O. 

Ppt.  Decomp.  in  air.  (Rimbach,  Z.  anorg. 
1907,  62.  413.) 

Potassium  iridicyanide,  K3Ir(CN)6. 
Easily  sol.  in  H2O. 

Silver    iridicyanide    ammonia,    Ag3Ir(CN)6, 

2NH3+3H2O. 

Ppt.  Decomp.  in  the  light.  (Rimbach,  Z. 
anorg.  1907,  52.  414.) 

Indium,  Ir. 

Insol.  in  all  acids,  including  aqua  regia, 
except  when  in  finely  divided  state,  as 
"iridium  black,"  when  it  is  sol.  in  aqua  regia. 
(Glaus,  J.  pr.  42.  251.) 

Iridium  ammonia  compounds. 
See— 
Chloriridicfo'amine  comps.,  ClIr(NH3)2X. 


Irido^namine 
Iridopeft/amine 

Iridoaquope  /famine 
Iridosoamine 
Iridosocfo'amine 

Ir(NH3)3X3. 
Ir(NH3)5X3. 
Ir(NH3)4X2. 
Ir(NH3)5(OH2)X3. 
Ir(NH3)2X2. 
'       Ir(NH3)4X2. 

Iridium  fribromide,  IrBr3+4H2O. 

Easily  sol.  in  H2O.  Insol.  in  alcohol  or 
ether.  (Birnbaum.) 

Iridium  tefrabromide,  IrBr4,  or  H2IrBr6. 

Deliquescent.     Sol.   in  H2O   and  alcohol. 
(Birnbaum.) 
See  Bromiridic  acid. 

Iridium     hydrogen     sesquibromide,     3HBr, 

IrBr3+H2O  =H3IrBr6+3H2O. 
See  Bromiridous  acid. 

Iridium  sesquibromide  with  MBr. 
See  Bromiridite,  M. 

Iridium  te^rabromide  with  MBr. 
See  Bromiridate,  M. 

Iridium  phosphorous  bromide,  IrBr3,  3PBr3. 

Partially  decomp.  by  H2O  into  a  sol.,  and 
insol.  modification.  Sol.  in  PBr3.  (Geisen- 
heimer.) 

IrBr3,  2PBr3.    Not  easily  attacked  by  H2O. 

IrBr4,  2PC13. 

See  Iridium  phosphorus  chlorobromide. 

Iridium  carbide,  IrC4(?). 

(Berzelius.) 

Stable  toward  H2O,  acids,  and  alcohol. 
(Strecker,  B.  1909,  42.  1773.) 


Iridium  wowochloride,  IrCl. 

Insol.  in  acids  and  bases.  (Wohler,  B. 
1913,  46.  1584.) 

Iridium  ^chloride,  IrCl2. 

Insol.  in  acids  and  bases.  (Wohler,  B. 
1913,  46.  1585.) 

Iridium  bichloride,  IrCl3. 

Insol.  in  acids  or  alkalies.  (Glaus,  C.  C. 
1861.  690.) 

Insol.  in  H2O,  acids  and  alkalies,  (Leidie, 
C.  R.  1899,  129.  1251.) 

+4H2O.    Sol.  inH2O.    (Claus.) 

Iridium  tefrachloride,  IrCl4,  or  H2IrCl6(?). 
Deliquescent,  and  easily  sol.  in  H2O. 

Iridium  ^'chloride  with  MCI. 
See  Chloriridite,  M. 

Iridium  tetmcbloride  with  MCI. 
See  Chloriridate,  M. 

Iridium  chloride  with  potassium  chloride  and 

sulphite. 
See  Chloriridosulphite,  potassium. 

Iridium  phosphorus  chloride,  IrP2Cl9. 

Insol.  in  cold  H2O.  SI.  decomp.  by  hot 
H2O.  (Geisenheimer,  A.  ch.  (6)  23.  254.) 

IrP2Clio.    Very  sol.  in  chloroform.    (G.) 

IrP3Cl12.  Easily  sol.  in  PC13,  or  CHC13, 
also  in  CS2  with  gradual  decomp.  SI.  sol.  in 
cold  H2O.  Decomp.  by  boiling  into  IrCl3, 
3H3PO4.  SI.  sol.  in  benzene,  ligroin  and  CC14. 
(Strecker,  B,  1909,  42.  1772.) 

+H2O.  Insol.  in  PC13  at  100°.  Very 
slowly  sol.  in  boiling  H2O.  (Geisenheimer,  A. 
ch.  (6)  23.  266.) 

IrP3Cl15.  Decomp.  by  H2O  into  2IrCl3, 
3H3PO3,  3H3PO4.  Violently  decomp.  by 
alcohol.  SI.  sol.  in  cold,  more  in  hot  POC13, 
without  decomp.  Very  sol.  in  PC13  with 
decomp.  into  IrP3Cli2;  similarly  in  PBr3.  Sol. 
in  AsCl3  with  combination.  Sol.  in  CS2  with 
decomp.  Sol.  in  SC12  with  combination. 
Easily  sol.  in  cold  CGH6  with  decomp.  Insol. 
in  CC14.  Sol.  in  CHC13  with  decomp.  (Gei- 
senheimer, A.  ch.  (6)  23.  254.) 

Iridium    phosphorus    arsenic    chloride, 
2IrP3Cl15,  5AsCl3. 

Sol.  in  H2O  with  decomp.  into  correspond- 
ing acid.  (Geisenheimer,  C.  R.  110.  1336.) 

IrCl3,  2PC13,  2AsCl3.  Very  sol.  in  H2O 
with  decomp.  Sol.  in  AsCl3;  insol.  in  CC14. 
( Geisenheimer . ) 

Iridium  phosphorus  sulphur  chloride,  IrCl3, 

2PC13,  2SC12. 

Very  sol.  in  si.  amt.  H2O,  with  decomp.  into 
an  acid  analogous  to  chlorophosphoiridic  acid. 
Sol.  in  SC12.  (Geisenheimer.) 


422 


IRIDIUM  PHOSPHORUS  CHLOROBROMIDE 


Iridium    phosphorus    chlorobromide,    IrBr4, 

2PC13. 
(Geisenheimer,  C.  R.  111.  40.) 

Iridium  ^hydroxide,  IrO2,  2H2O  =  IrO4H4. 

Insol.  in  dil.  HNO3,  or  H2SO4+Aq.  Slowly 
but  completely  sol.  in  HCl-j-Aq.  Sol.  in 
KOH,  and  NaOH+Aq.  (Glaus,  J.  pr.  39. 
104.) 

Iridium  sesqmhy  dioxide,  Ir2O6H6. 

Not  attacked  by  acids,  except  slightly  by 
cone.  HCl+Aq.  (Glaus,  C.  C.  1861.  690.) 

Iridium  friiodide,  IrI3. 

Very  si.  sol.  in  cold,  somewhat  more  in  hot 
H2O.  Insol.  in  alcohol.  (Oppler.  J.  B.  1857. 
263.) 

Iridium  tetraiodide,  IrI4. 

Insol.  in  H2O  or  acids.    (Lassaigne.) 
Sol.  in  solutions  of  iodides.    (Oppler.) 

Iridium  Zn'iodide  with  MI. 
See  lodiridite,  M. 

Iridium  tetraiodide  with  ML 
See  lodiridate,  M. 

Iridium  dioxide,  IrO2. 

Very  si.  sol.  in  acids. 

Freshly  pptd.  Sol.  in  cone.  H2SO4,  hot 
2-N  H2SO4,  HNO3,  HC1.  Insol.  in  2-N  KOH 
and  si.  sol.  in  hot  1-N  KOH. 

Dried  in  a  dessicator.  Sol.  in  HC1.  Insol. 
in  H2SO4,  HNO3  and  KOH. 

Dried  at  100°.  Sol.  in  hot  cone.  HC1. 
Insol.  in  H2SO4,  HNO3  and  KOH.  (Wohler, 
Z.  anorg.  1908,  67.  334.) 

See  also  Iridium  dihy  dioxide. 

Iridium  trioxide,  IrO3. 

Unstable.  (Wohler,  Z.  anorg.  1908,  67. 
340.) 

Iridium  sesquioxidet  Ir2O3. 

Insol.  in  acids. 

Sol.  in  cone.  H2SO4,  and  hot  cone.  HC1. 
Forms  colloidal  solution  with  dil.  HC1.  Cone. 
HNO3  converts  it  into  the  dioxide. 

Insol.  in  KOH+Aq.  (Wohler,  Z.  anorg. 
1908,  57.  339.) 

Iridium  oxybromide,  Ir3Br8O2=2IrBr4,  IrO2. 
Not  decomp.  by  H2O.     (Geisenheimer,  A. 
ch.  (6)  23.  286.) 

Iridium  phosphide,  Ir2P. 

(Clarke  and  Joslin,  Am.  Ch.  J.  6.  231.) 

Iridium  sesgwselenide,  Ir2Se3. 

Insol.  in  HNO3;  slowly  sol.  in  hot  aqua 
regia.  (Chabrie"  and  Bouchonnet,  C.  R.  1903, 
137.  1060.) 


Iridium  raonosulphide,  IrS. 

Inso!.  in  HNO3-f-Aq,  and  very  si.  sol.  if 
at  all  in  aqua  regia.  (Berzelius.) 

Sol.  in  K2S,  and  KSH+Aq. 

+zH2O.  SI.  sol.  in  H2O;  sol.  in  cold 
HNO3+Aq.  Insol.  in  NH4Cl+Aq  or  dil. 
acids.  More  sol.  in  K2S+Aq  than  PtS2. 
(Berzelius.) 

Iridium  ^sulphide,  IrS2. 

Not  attacked  by  H2O,  but  decomp.  when 
exposed  moist  in  air.  Not  Attacked  by  sat. 
HCl+Aq  or  by  cone.  HNO3+Aq,  but  is 
oxidised  by  fuming  HNO3+Aq,  and  aqua 
regia.  Insol.  in  NH4  sulphides,  or  polysul- 
phides+Aq.  Slowly  sol.  in  alkali  polysul- 
phides-f  Aq.  (Antony,  Gazz.  ch.  it.  23,  1. 
190.) 

Iridium  sesgm'sulphide,  Ir2S3. 

SI.  sol.  in  H2O.    Sol.  in  HNO3,  or  K2S+Aq. 

IridoJnamine  chloride,  Ir(NH3)3Cl3. 

SI.  sol.  in  H2O.  Not  attacked  by  boiling 
H2SO4.  (Palmaer,  B.  22.  15.) 

Irido^raamine  chloride,  Ir(NH3)4Cl3. 
Very  sol.  in  H2O.    (Palmaer,  B.  22.  15.) 

chlorosulphate,[Ir(NH3)4Cl2]S04  + 

4H2O. 
(Palmaer.) 

Iiidopentamme  bromide,  Ir(NH3)6Br3. 

Sol.  in  352  pts.  H2O  at  12.5°.  (Palmaer,  B. 
23.  3817.) 

bromochloride,  Ir(NH3)5ClBr2. 

Sol.inH2O.    (Palmaer,  B.  24. 2090.) 

bromonitrite,  Ir(NH3)6Br(NO2)2. 

Sol.  in  17.9  pts.  H2O  at  18°.    (Palmaer.) 

bromosulphate,  Ir(NH3)5BrSO4+H2O. 

Sol.  in  H2O.    (Palmaer.) 

carbonate,  [Ir(NH3)5]2(C03)3+3H2O. 

Sol.  in  H2O.    (Glaus,  J.  pr.  63.  99.) 

^chloride,  Ir(NH3)6Cl3. 

Sol.  in  153.1  pts.  H2O  at  15.1°,  (Palmaer, 
B,  23.  3810.) 

Sol.  in  hot  H2O  containing  HC1.  (Glaus,  J. 
pr.  69.  30.) 

chlorobromide,  Ir(NH3)5ClBr2. 

Sol.  in  213.6  pts.  H2O  at  15°.    (Palmaer.) 

chloroiodide,  Ir(NH3)6ClI2. 

Sol.  in  104.5  pts.  H2O  at  15°.    (Palmaer.) 

chlorooxalate,  Ir(NH3)5ClC2O4. 

SI.  sol.  in  H2O.    (Palmaer.) 


IRON 


423 


Iridopentamine  chloronitrate, 

Ir(NH3)6Cl3N03)2. 
Sol.  in  51.54  pts.  H2O  at  15.4°.    (Palmaer.) 

chloronitrite, 

Ir(NH3)5Cl(N02)2. 
Easily  sol.  in  H2O.    (Palmera.) 

chloroplatinate,  Ir(NH3)5Cl3,  PtCl4. 

Very  si.  sol.  in  H2O.    (Palmear.) 

chlorosulphate,  Ir(NH3)5ClSO4+2H2O. 

Sol.  in  134.5  pts.  H2O  at  15°.    (Palmaer.) 

hydroxide,  Ir(NH3)5(OH)3. 

Known  only  in  solution,  which  decomp.  on 
evaporation.  (Glaus.) 

nitrate,  Ir(NH3)5(NO3)3. 

Moderately  sol.  in  H2O.    (Glaus.) 

Sol.  in  349  pts.  H2O  at  16°.    (Palmaer.) 

sulphate,  [Ir(NH3)6]2(SO4)3. 

Sol.  in  H2O.    (Glaus.) 

Iridoaquopentfamine  bromide, 

Ir(NH3)5(OH2)Br3. 

Sol.  in  4  pts.  H2O.  Pptd.  from  aqueous 
solution  by  HBr+Aq.  (Palmaer,  B.  24. 
2090.) 

chloride,  Ir(NH3)6(OH2)Cl3. 

Sol.  in  1.2  to  1.5  pts.  H2O  at  ord.  temp. 
Pptd.  by  HCl+Aq  from  aqueous  solution. 
(Palmaer,  B.  24.  2090.) 

nitrate,  Ir(NH3)5(OH2)(NO3)3. 

Sol.  in  about  10  pts.  H2O  at  17°.  Pptd. 
from  aqueous  solution  by  HNO3+Aq.  (Pal- 
maer.) 

Iridonitrous  acid,  H6Ir2(NO2)i2. 

Easily  sol.  in  H2O.    (Gibbs,  B.  4.  281.) 

Ammonium  iridonitrite,  (NH4)eIr2(NO2)i2. 

Almost  insol.  in  cold  H2O;  decomp.  by  hot 
H2O  with  evolution  of  N2.  Decomp.  by  hot 
cone.  H2SO4  or  HC1.  Insol.  in  sat.  NH4C1+ 
Aq.  (Leidie,  C.  R.  1902,  134.  1583.) 

Barium  iridonitrite  iridochloride, 

Ba3Ir2(NO3)12,  Ba3Ir2Cli2. 
Sol.  in  H2O.    (Lang.) 

Mercuric  iridonitrite,  Hg3Ir2(NO2)i2. 
Insol.  in  H2O.    (Gibbs,  B.  4.  280.) 

Potassium  iridonitrite,  K6Ir2(NO2)i2. 

SI.  sol.  in  cold,  more  sol.  in  boiling  H2O. 
Decomp.  by  hot  HC1  or  H2SO4.  Insol.  in 
KCl+Aq.  (Leidie,  Bull.  Soc.  1902,  (3)  27. 
937.) 

+2H2O.    Moderately  sol.  in  H2O. 


Potassium  iridonitrite  iridochloride, 

K6Ir2(N02)12,  K6Ir2Cl12. 
Sol.  in  H2O. 

Silver  iridonitrite,  Ag6Ir2(NO2)i2. 

Difficultly  sol.  in  cold,  more  easily  in  hot 
H20. 

Sodium  iridonitrite,  Na6lr2(NO2)i2+2H2O. 

SI.  sol.  in  H2O.  Sol.  in  cold  H2O.  Decomp. 
by  hot  cone.  H2SO4  or  HC1.  (LeidiS,  C.  R. 
1902,  134.  1583.) 

Sodium  iridonitrite  iridochloride, 

Na4Ir2Cl2(N02)8+2H2O. 
SI.  sol.  in  H2O.    (Gibbs.) 
Na6lr2(NO2)i2,  NaJraCle.    Insol.  in  cold,  si. 
sol.  in  hot  H20.    (Lang.) 

Iridosamine  chloride,  Ir(NH3)2Cl2. 

Nearly  insol.  in  H2O.  (Skoblikoff,  A.  84. 
275.) 

sulphate,  Ir(NH3)2SO4. 

Easily  sol.  in  H2O.    (Skoblikoff.) 

Iridosodiamine  chloride,  Ir(N2H6)2Cl2. 

Insol.  in  cold,  decomp.  by  hot  H2O.  (Skob- 
likoff.) 

-  nitrate,  Ir(N2H6NO3)2. 
Easily  sol.  in  H2O.    . 

sulphate,  Ir(N2H6)2SO4. 

SI.  sol.  in  cold,  easily  in  boiling  H2O.  SI., 
sol.  in  alcohol. 

Irido sulphuric  acid. 

Potassium  iridosulphate,  K6Ir2(SO4)6. 

Sol.  in  H2O.  (de  Boisbaudran,  C.  R.  96. 
1406.) 

Iridosulphurous  acid. 

Ammonium  iridosulphite,  (NH4)6Ir2(SO8)6+ 

6H2O. 

Slightly  sol.  in  H2O.  (Birnbaum,  A.  136. 
179.) 

Potassium  iridosulphite,  K6Ir2(SO3)6+6H2O. 
Slightly  sol.  in  H2O. 

Sodium  iridosulphite,  Na6lr2(SO3)6+8H2O. 
Scarcely  sol.  in  H2O. 

Iron,  Fe. 

Permanent  in  dry  air;  oxidises  only  slowly 
in  moist  air,  but  rapidly  when  in  contact 
with  air  and  H2O  simultaneously. 

Fe  does  not  rust  in  contact  with  air  and 


424 


IRON 


H2O  containing  alkalies  even  in  very  small 
amounts.  (Payen,  A.  ch.  50.  305.) 

Not  attacked  at  ord.  temp,  by  H2O  free 
from  air.  More  easily  oxidised  by  NH4  salts 
-j-Aq  than  by  H2O  when  exposed  to  air 
simultaneously.  (Persoz,  A.  ch.  (3)  24.  506.) 

Iron  is  slowly  attacked  by  distilled  H2O  in 
presence  of  air.  100  ccm.  distilled  water  re- 
moved 29  mg.  from  11.8  sq.  cm.  iron  in  one 
week,  while  air  free  from  CO2  was  passed 
through  the  solution.  In  presence  of  CO2,  54 
mg.  were  removed.  (Wagner,  Dingl.  221. 
260.) 

CO2  acts  as  a  catalyst  for  the  solution  of 
Fe  by  H2O.  (Whitney,  J.  Am.  Chem.  Soc. 
1903,  25.  394.) 

Iron  is  most  easily  oxidised  when  it  is  ex- 
posed to  air,  and  H2O  is  deposited  on  it  at  the 
same  time  in  liquid  form. 

100  1.  sea  water  dissolve  27.37  g.  from  1  sq. 
metre  Fe;  29.16  g.  from  1  sq.  metre  steel; 
1.12  g.  from  1  sq.  metre  galvanised  Fe.  (Cal- 
vert  and  Johnson,  C.  N.  11).  171.) 

Readily  sol.  in  HC1,  dil.  H2SO4+Aq,  and 
most  other  acids. 

Action  of  H2SO4+Aq  (1:12)  is  very  much 
accelerated  by  a  few  drops  of  PtCl4+Aq;  the 
addition  of  As2O3  arrests  the  action  com- 
pletely. Tartar  emetic  and  HgCl2  diminish 
the  action,  but  do  not  arrest  it.  CuSO4-|-Aq 
strongly  accelerates  the  action,  and  Ag2SO4  + 
Aq  also  to  a  less  extent. 

In  the  case  of  HCl+Aq,  the  addition  of 
small  amts.  of  metallic  salts  also  influences 
the  action.  Weak  HC2H3O2+Aq  has  but 
little  action,  and  the  addition  of  PtCl4  in- 
creases it;  As2O3  stops  it;  other  solutions  have 
no  effect.  With  racemic  and  tartaric  acids 
the  phenomena  are  the  same. 

With  oxalic  acid,  PtCl4  prevents  the  action. 
Saline  solutions  and  even  distilled  H2O,  when 
mixed  with  PtCl4,  have  slight  solvent  action. 
(Millon,  C.  R.  21.  45.) 

Above  phenomena  are  due  to  galvanic  ac- 
tion from  metal  deposited  on  the  iron. 
(Barreswill,  C.  R.  21.  292.) 

H2SO4  has  only  si.  action  on  cast-iron  at 
ord.  temp,  with  exclusion  of  air. 

Weak  acids  have  a  strong  action  at  higher 
temperatures. 

Charcoal  pig-iron,  and  case-hardened  cast- 
iron  are  much  less  attacked  by  weak  acids  at 
b.-pt.  than  other  sorts  of  Fe.  Scotch  pig-iron 
is  most  strongly  attacked. 

99.8%  H2SO4  has  very  si.  action  on  iron  at 
ord.  temp,  when  air  is  excluded.  (Lunge, 
Dingl.  261.  131.) 

Resistance  against  dil.  H2SO4+Aq  is 
greatly  increased  by  increase  in  amt.  of  C  if 
chemically  combined,  less  so  by  P  or  Si. 
(Ledebur,  Dingl.  223.  326.) 

Passive  Iron. — When  Fe  is  treated  with 
pure  cone.  HNO3+Aq  of  1.512-1.419  sp.  gr., 
it  soon  becomes  coated  with  a  bluish  or  black 
coating,  apparently  FeO,  and  when  thus 


covered  Fe  is  not  attacked  by  HNO3+Aq  of 
any  strength  at  ord.  temp,  or  at  the  temp, 
of  a  freezing  mixture;  but  action  occurs  on 
heating.  Nor  is  Fe  attacked  at  ord.  temp, 
by  acid  of  1.401  sp.  gr.  or  even  somewhat 
weaker  acid,  though  action  begins  at  once 
on  heating.  Very  dil.  HNO3+Aq  attacks 
Fe  at  ord.  temp,  with  formation  of  NH4NO3 
and  Fe(NO3)2.  The  action  of  HNO3+_Aq  is 
influenced  by  PtCl4.  If  acid  containing  4.5 
equivalents  of  H2O  is  diluted  with  2-3  vols. 
H2O,  and  then  poured  on  Fe  turnings,  they 
dissolve  at  once  with  evolution  of  nitrous 
fumes  and  formation  of  ferric  salt,  but  if  to 
the  acid  one  drop  of  PtCl4  be  added,  only 
H  gas  is  evolved,  and  NH4NO3  and  Fe(NO3)2 
are  formed.  (Millon,  C.  R.  21.  47.) 

The  more  H2O  the  acid  contains  the  lower 
will  be  the  temp,  at  which  the  Fe  remains 
passive.  Shaking  the  wire  hastens  the  pas- 
sivity. Contact  with  Pt,  Au,  or  C  does  not 
prevent  it.  Fe  wire  becomes  passive  by  re- 
maining 10  min.  in  HNO3  vapour.  (Renard, 
C.  R.  79.  159.) 

Iron  may  be  made  passive  by  HC1O3, 
HBrO3,  HIO3,  H2CrO4,  in  the  same  way  as 
by  HNO3. 

Iron  may  also  be  made  passive  by  moderate 
ignition. 

Passivity  occurs  with  HNO3+Aq  of  1.38 
sp.  gr.  after  a  short  time  at  31°;  but  if  temp,  is 
32°,  passivity  does  not  occur. 

Colourless  HNO3+Aq  of  1.42  sp.  gr.  pro- 
duces passivity  at  55°  but  not  at  56°.  Red 
fuming  HNO3+Aq  of  1.42  sp.  gr.  produces 
passivity  at  82°  but  not  at  83°.  (Ordway, 
Sill.  Am.  J.  (2)  40.  316.) 

The  passivity  of  Fe  is  destroyed  when  it  is 
placed  in  a  magnetic  field  at  a  much  lower 
temperature  than  when  in  normal  condition. 
(Nichols  and  Franklin,  Sill.  Am.  J.  (3)  34. 
419.) 

Passivity  depends  on  a  coating  of  NO  which 
hinders  the  action  of  the  acid.  All  operations 
which  remove  this  layer  terminate  the  pas- 
sivity, as  shaking,  rubbing,  placing  in  a 
vacuum,  etc.  (Varenne,  C.  R.  89.  783.) 

When  Fe  is  plunged  in  HNO3+Aq  of  1.42 
sp.  gr.  there  is  a  sudden  evolution  of  gas  which 
ceases  after  3  to  20  seconds,  and  the  surface 
becomes  bright.  The  same  phenomena  take 
place  with  a  more  dilute  acid,  if  of  not  less 
than  1.32  sp.  gr.  In  the  latter  case,  there  is 
an  immediate  evolution  of  gas,  which  sud- 
denly ceases  and  the  metal  becomes  bright, 
but  soon  the  acid  begins  to  act  again  at  a 
single  point,  and  the  action  gradually  spreads 
over  the  whole  surface;  this,  however,  soon 
ceases  again,  and  we  have  an  "intermittent 
passivity." 

If  a  part  of  a  piece  of  iron  is  immersed  in 
strong  acid,  the  whole  of  it  is  made  passive. 
This  is  explained  by  the  NO  spreading  over 
the  whole  surface  by  capillarity. 

The  passivity  ceases  when  the  Fe  is  placed 
in  dil.  acid,  after  a  longer  or  shorter  time, 


IRON  BORIDE 


425 


according  to  the  dilution  of  the  acid, — when 
the  acid  has  sp.  gr.  =  1.30,  after  11  days 

((  (f  ((  I    OO         ti  K         (( 

L26      "     32  hours 
it         it  (i        j  16      (i     12      it 

Iron  may  also  be  made  passive  by  long 
standing  in  NO  gas  under  pressure.  ( Varenne, 
C.  R.  90.  998.) 

Fe  is  made  passive  by  a  coating  of  Fe3O4, 
not  by  NO.  (Schonbein,  Pogg.  39.  342.) 
(Beetz,  Pogg.  67.  286.)  (Ramann,  B.  14. 
1430.) 

Passivity  may  also  be  caused  by  NH4NO3 
+Aq,  ammoniacal  AgNO3-fAq,  Fe(NO3)3, 
Fe(N03)2,  A1(N03)3,  Co(NO3)2,  Ni(NO3)2, 
etc.+Aq  instead  of  HNO3+Aq.  (Ramann. 

B.  14.  1933.) 

Hardly  attacked  by  either  dil.  or  cone,  acids 
when  they  are  under  high  pressure.  (Cailletet 

C.  R.  68.  395.) 

Iron  is  dissolved  by  HNO3+Aq,  even  when 
very  cone.,  but  no  gas  is  evolved  and  the  pro- 
cess is  very  slow. 

HNO3+Aq  of  the  following  sp.  gr.  dissolves 
the  given  amts.  from  strips  of  pure  Fe. 


Sp.  gr.  of  acid 

Diminution  of  weight  in 
24  hours 

1.28 
1.34 
1.38 
1.48 
1.53 

0.82% 
0.75 
0.29 
0.34 
5.80 

(Gautier  and  Charpy,  C.  R.  113.  1451.) 

Insol.  in  liquid  chlorine  below  90°.  (Lange, 
Zeit.  angew.  Ch.  1900,  13.  686.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  ch.  J. 
1898,  20.  828.) 

Not  attacked  by  alkalies. 

Sol.  in  NaOH+Aq  (34%)  when  air  is  blown 
through  the  liquid.  (Zirnite,  Ch.  Ztg.  12. 
355.) 

NaOH+Aq  attacks  iron  and  steel.  (Vena- 
tor, Dingl.  261.  133.) 

NaOH  -f- Aq  has  slight  action  on  Fe  between 
15°  and  100°.  (Lunge,  Dingl.  261.  131.) 

Presence  of  alkalies  prevent  rusting  en- 
tirely, and  fats  and  oils  greatly  hinder  it. 
(Wagner.) 

Sol.  in  alkali  hydrogen  carbonates +Aq. 
(Berzelius.) 

Sat.  NaCl+Aq  has  si.  but  perceptible  ac- 
tion on  Fe.  NH4Cl+Aq  has  stronger  action 
than  NaCl+Aq.  (Lunge.) 

100  ccm.  H2O  containing  0.5  g.  NaCl  or 
KC1  removed  42  mg.  from  11.8  sq.  cm.  iron 
in  one  week,  while  air  free  from  CO2  was 
passed  through  the  solution,  and  72  mg.  in 
presence  of  CO2. 

100  ccm.  H2O  containing  1  g.  NH4C1  re- 
moved 45  mg.,  and  76  mg.  respectively  under 
the  above  conditions. 

100  ccm.  H2O  containing  0.8  g.  MgCl2  re- 


moved 49  mg.,  and  65  mg.  respectively  under 
the  above  conditions. 

Not  attacked  by  100  ccm.  H2O  containing 
1  g.  Na2CO3,  or  by  CaO2H2+Aq.  (Wagner, 
Dingl.  221.  260.) 

Action  of  KClO3+Aq.  KClO3+Aq  (6.3% 
KC1O3)  oxidised  11.21  g.  cast  iron  and  20.1  g. 
pure  iron  from  a  surface  of  1  sq.  metre  in  7 
hours;  KClO3+Aq  (25%  KC1O3)  oxidised 
24.59  g.  cast,  and  44.90  g.  pure  Fe  under 
above  conditions;  Ca(ClO3)2,  CaCl2+Aq  (20° 
Baume)  obtained  by  passing  Cl  through 
CaO2H2+Aq  oxidised  85  g.  cast,  and  95  g. 
pure  Fe  under  the  above  conditions.  (Lunge 
and  Deggeler,  J.  Soc.  Chem.  Ind.  4.  32.) 

Easily  sol.  in  organic  acids. 

Comparative  action  of  oils  on  Fe. 


Amount  Fe  dissolved 

Neatsfoot  oil 

0.0875  grains 

Colza          " 

0.0800 

Sperm 

0.0460 

Lard 

0.0250 

Olive 

0.0062 

Linseed       " 

0.0050 

Seal 

0.0050 

Castor        " 

0.0048 

Paraffine    " 

0.0045 

Almond      " 

0.0040 

"Lubricating"  oil 

0.0018 

(Watson,  C.  N.  42.  190.) 

l/£  p.c.m    nlpin  a.niH  Hissolvps  0  0097  e\  FP  in 

6  days.  (Gates,  J.  phys.  Chem.  1911,  15. 
143.) 

Fe  dissolves  in  albumen  solution  to  the 
extent  of  1  to  2  per  cent.  (Buchner,  Arch. 
Pharm.  (3)  20.  417.) 

Attacked  by  sugar +Aq  at  115-120°,  also 
by  inverted  sugar  or  malt  extract,  not  by 
glycerine  or  mannite+Aq.  (Klein  and  Berg, 
C.  R.  102.  1170.) 

Iron  arsenide,  FeAs2. 

Min.  Lollingite.  Sol.  in  HNO3+Aq  with 
separation  of  As2O3. 

Fe3As4.    Min.  Leucopyrite. 

Iron  arsenide  sulphide,  FeAs2,  FeS2. 

Min.  Arsenopyrite.  Sol.  in  HNO3+Aq 
with  separation  of  S  and  As2O3;  wholly  sol. 
in  aqua  regia;  not  attacked  by  HCl+Aq. 

Iron  boride,  Fe2B. 

Decomp.  by  H2O.  Sol.  in  hot  dil.  HC1  or 
H2SO4  and  in  hot  cone.  HC1  or  H2SO4.  Sol. 
in  hot  dil.,  or  cold  cone.  HNO3.  (Jassonneix, 
C.  R.  1907,  146.  122.) 

FeB.  Sol.  in  molten  alkali  carbonates;  not 
sol.  in  dil.  or  cone.  H2SO4  in  the  cold;  sol.  in 
boiling  H2SO4  and  in  HNO3.  (Moissan,  Bull. 
Soc.  1895,  (3)  13.  958.) 

Stable  in  dry  air.    Decomp.  by  aqua  regia, 


426 


IRON  BROMIDE 


but  not  readily  sol.  in  cone.  H2SO4  and  HC1. 
(Moissan,  C.  R.  1895,  120.  176.) 

FeB2.  Decomp.  by  H2O.  Sol.  in  HNO3 
and  in  hot  cone.  HC1.  (Jassonneix,  C.  R. 
1907,  145.  122.) 

Iron  (ferrous)  bromide,  FeBr2. 

Sol.  in  H2O.     Decomp.  by  heating  on  air. 
Sat.  FeBr2+Aq  contains  at: 
—21°         —7°         +10°         21° 
47.0        48.3        52.3        53.7%FeBr2, 

37°  50°  65°  95° 

56.0        58.0        59.4        63.3%FeBr2. 
(Etard,  A.  eh.  1894,  (7)  2.  541.) 

+4H2O.  Very  sol.  in  H2O;  pptd.  from 
cooled  aq.  solution.  (Volkmann,  C.  C.  1894, 
II.  611.) 

+6H2O.    Sol.  in  H2O.    (Lowig.) 

+9H2O.    (Volkmann.) 

Ferric  bromide,  FeBr3. 

Deliquescent.  Sol.  in  H2O,  alcohol,  and 
ether.  (Lowig.) 

SI.  sol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

+6H2O.  Sol.  in  alcohol  and  ether.  (Bol- 
schakoff,  C.  C.  1898,  II.  660.) 

Ferrous  mercuric  bromide. 

Deliquescent,    (v.  Bonsdorff.) 
Ferric  rubidium  bromide,  Rb2FeBr6+H2O. 

Sol.  in  H2O.  (Walden,  Z.  anorg.  1894,  7. 
332.) 

Ferrous  stannic  bromide. 

See  Bromostannate,  ferrous. 
Ferrous  bromide  nitric  oxide,  3FeBr2,  2NO. 

Sol.inH2O.  Not  isolated.  (Thomas,  C.  R. 
1896,  123.  944.) 

Ferric  bromochloride,  FeCl2Br. 

Very  deliquescent,  and  sol.  in  H2O,  alcohol, 
and  ether.  Notably  sol.  in  chloroform,  ben- 
zene, and  toluene.  Insol.  in  CS2.  (Lenor- 
mand,  C.  R.  116.  820.) 

Iron  carbide,  Fe8C. 

(Gurlt,  J.  B.  1856,  781.) 

Mixture  of  Fe  and  FeC4.  (Tunner,  Polyt. 
Centralbl.  1861.  1227.) 

Fe4C.    (Karsten,  J.  pr.  40.  229.) 

Fe3C.  Sol.  in  hot  cone.  HC1;  oxidized 
slowly  by  moist  air.  (Campbell,  Am.  Ch.  J. 
1896,  18.  840-841.) 

Fe2C2.    (Rammelsberg,  C.  C.  1847.  60.) 

Iron  molybdenum  carbide,  Fe3C,  Mo2C. 

Sol.  in  hydracids;  insol.  in  HNO3.  (Wil- 
liams, C.  R.  1898,  127.  484.) 

Iron  tungsten  carbide,  2Fe3C,  3W2C. 

Insol.  in  H2O  and  hydracids;  sol.  in  HNO3 
and  H2SO4.  (Williams,  C.  R.  1898,  127. 
411.) 


Iron  carbonyl,  Fe(CO)5. 

Slowly  decomp.  on  air.  Not  attacked  by 
dil.  H2SO4,  HNO3,  or  HCl+Aq.  Cone.  HNO3, 
Cl2+Aq,  or  Br2+Aq  decomp.  easily.  Sol.  in 
alcoholic  solution  of  KOH  or  NaOH  with  sub- 
sequent decomp.  Sol.  in  alcohol,  ether, 
benzene,  mineral  oils,  etc.  (Mond  and  Lan- 
ger,  Chem.  Soc.  59.  1090.) 

Fe2(CO)7.  Decomp.  on  air.  Not  attacked 
by  H2SO4  or  HCl+Aq.  Sol.  in  alcoholic 
potash.  Very  much  less  sol.  in  organic  sol- 
vents than  Fe(CO)5.  (Mond  and  Langer.) 

Ferrous  chloride,  FeCl2. 

Deliquescent.     Easily   sol.    in   H2O    with 

evolution  of  heat,  or  in  alcohol.     Insol.  in 

ether.    (Jahn.) 

Sol.  in  2  pts.  H2O  at  18.75°.    (Abl.) 
Sol.  in  1  pt.  strong  alcohol.    (Wenzel.) 

Sp.  gr.  of  FeCl2=Aq  at  15.5°. 


Sp.  gr. 

%  FeCh 

%  FeCh,  4H20 

1.05 

5.40 

8.45 

1.06 

6.43 

10.09 

1.07 

7.47 

11.69 

.08 

8.48 

13.29 

.09 

9.49 

14.86 

.10 

10.47 

16.41 

.11 

il.45 

17.86 

.12 

12.42 

19.46 

.13 

13.37 

20.96 

.14 

14.31 

22.41 

.15 

15  24 

23.87 

.16 

16.15 

25.31 

.17 

17.05 

26.73 

.18 

17.94 

28.13 

.19 

18.83 

29.51 

.20 

19.68 

30.85 

.21 

20.50 

32.14 

.22 

21.39 

33.53 

.23 

22.24 

34.84 

.24 

23.05 

36.11 

.25 

23.86 

37.38 

.26 

24.68 

38.67 

.27 

25.44 

39.87 

.28 

26.19 

41.04 

.29 

26.98 

42.29 

.30 

27.75 

43.49 

.31 

28.49 

44.65 

.32 

29.23 

45.81 

.33 

29.96 

46.94 

1.34 

30.68 

48.08 

1.35 

31.39 

49.18 

1.36 

32.10 

50.30 

1.37 

32.79 

51.39 

1.38 

33.47 

52.46 

1.39 

34.14 

53.50 

1.40 

34.80 

54.55 

1.41 

35.46 

55.57 

1.42 

36.09 

56.56 

1.43 

36.73 

57.55 

1.44 

37.33 

58.51 

(Dunn,  J.  So< 

3.  Chem.  Ind.  1 

902,  21.  390.) 

IRON  CHLORIDE 


427 


Insol.  in  liquid  HF.  (Franklin,  Z.  anorg. 
1905,  46.  2.) 

Sol.  in  acetone;  insol.  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

Sol.  in  acetone.  (Naumaim,  B.  1904,  37. 
4328.) 

SI.  sol.  in  methyl  acetate.  (Naumann,  B. 
1909,42.3790.) 

Sol. .in  ethyl  acetate.  (Naumann,  B.  1910, 
43.  314.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1904,  37.  3601.) 

Yellow  modification  is  sol.  in  benzonitrile. 
(Naumann,  B.  1914,  47.  1369.) 

Mol.  weight  determined  in  pyridine.  (Wer- 
ner, Z.  anorg.  1897,  16.  21.) 

+2H2O.    (Jonas.) 

+4H2O.  Deliquescent.  Easily  sol.  in 
alcohol.  Sol.  in  0.68  pt.  cold  H2O.  (Reimann, 
Mag.  Pharm.  17.  215.) 

Sat.  aq.  solution  contains  at: 
16°        18°         25°         28°        43° 
40.5      40.9       41.0       42.5      44.4%FeCl2, 

50°      53°       72°       89°       96°  118° 
45.0  45.9    49.2    51.3    51.0  51.7%FeCl2. 
(fitard,  A.  ch.  1894,  (7)  2.  537.) 

100  g.  FeCl2,  4H2O+Aq  contain  17.54  g. 
Fe  at  22.8°;  18.59  g,  at  43.2°.  (Boecke, .  N. 
Jahrb.  Min.  1911,  I,  61.) 


More  sol.  in  water  containing  NO  than  in 
pure  H2O.  (Gay,  Bull.  Soc.  (2)  44.  175.) 

Sol.  in  hot  HCl+Aq.  (Sabatier,  Bull.  Soc. 
1895,  (3)  13.  599.) 

[Sabatier  could  not  obtain  FeCl2+6H2O  of 
Lescceur.] 

Ferroferric  chloride,  Fe3Cl8+18H2O. 

Deliquescent.     (Lefort,  J.  Pharm.  (4)  10. 

85.) 

Ferric  chloride,  Fe2Cl6  or  FeCl3. 

Very  deliquescent,  and  sol.  in  H2O  with 
evolution  of  great  heat. 

100  mols.  H2O  dissolve  mols.  anhydrous 
Fe2Cl6  at  t°. 


t° 

Mols.  FezCle 

t° 

Mols.  FeaCle 

66 
70 
75 

29.20 
29.42 
28.92 

80 
100 

29.20 
29.75 

(Roozeboom,  Z.  phys.  Ch.  10.  477.) 

See  also  hydrated  salts  below. 

Solution  in  H2O  is  decomp.  into  colloidal 
Fe2O3,  zH2O  and  HC1,  upon  heating  if  cone., 
and  on  simple  standing  if  dil. 


Krecke  (J.  pr.  (2)  3.  286)  gives  the  following  table. 


%  Fe2Cl6  in 
solution 

Temp,  at  which  Graham's 
colloidal  hydrate  is  formed 

Temp,  at  which 
Saint  Gilles' 
colloidal  hy- 
drate is  formed 

Temp,  at  which 
oxychlorides  are 
formed 

Temp,  at  which 
FeaOs  is  formed 

32 

100-130° 

100°  + 

140° 

16 

100-120 

Fe2Cl6  re- 

. .  . 

" 

120 

8 

100-110 

formed  on 

" 

110 

4 

90-100 

cooling. 

90 

2 

87 

87 

1 

83 

i(XM30° 

.  .  . 

0.5 

75 

Fe2Cl6  not 

a 

.... 

.  .  . 

0.25 

64 

reformed 

it 

... 

0.125 

54 

on  cooling. 

" 

.  .  . 

0.0625 

36 

" 

Sp.  gr.  of  Fe2Cl6+Aq. 

% 
Fe2Cl6 

Sp.  gr. 

at  4.8° 

Sp.  gr. 
at  9.7° 

Sp.  gr. 
at  14.6° 

Sp.  gr. 
at  19.7° 

49.61 

1.5609 

1  .  5575 

1.5540 

1  .  5497 

41.00 

1.4413 

1.4387 

1.4361 

1.4335 

36.95 

1.3847 

1  .  3824 

1.3800 

33.25 

1^3381 

1.3359 

1.3339 

1.3317 

24.60 

1.2351 

1.2334 

1.2318 

1.2298 

22.54 

1.2140 

1.2129 

1.2107 

1.2090 

16.79 

1  .  1534 

1  .  1521 

1  .  1507 

1.1491 

10.45 

1.0939 

1.0930 

1.0918 

1.0901 

4.65 

1.0382 

2.70 



1.0221 

(Schult,  from  Gerlach,  Z.  anal.  27.  278.) 

Sp.  gr.  of  Fe2Cl6+Aq  increases  or  diminishes 
between  8°  and  24°  for  a  decrease  or  in- 
crease of  temp,  of  1°  by  the  following 
amts. 


%  Fe2Cl6 

Corr. 

%  FesCle 

Corr. 

50-60 
45-49 
40-44 

0.0008 
0.0007 
0.0006 

30-39 
20-29 
10-19 

0.0005 

0.0004 
0.0003 

(Hager,  1.  c.) 


428 


IRON  CHLORIDE 


Sp.gr.  of  Fe2Cl6+Aq  at  17.5°.    ' 

Solubility  of  Fe2Cl6  in  HCl+Aq. 

ji 

-2? 

_s 

Sat.  solution  contains 

CD 

Sp.  gr. 

£\^sl 

Sp.  gr. 

k\  ^ 

Sp.  gr. 

per  100  mols.  H2O 

fe 

LXJ 

^ 

t° 

Solid  phase 

mols.  HC1 

mols. 
Fed  3 

1 

1.0073 

1f\t  AC* 

21 

1  .  1644 

41 

1.3746 

3 

.0146 
1.0219 

22 
23 

.  1746 

.1848 

42 
43 

1  .  3870 
1.3994 

30 

0 

12.70 

4 

1.0292 

24 

.1950 

44 

1.4118 

" 

5.92 

16.07 

5 

1.0365 

25 

.2052 

45 

1.4242 

tt 

0 

20.90 

6 

1  .  0439 

26 

.2155 

46 

1.4367 

25 

0 

10.90 

7 

1.0513 

27 

.2258 

47 

1.4492 

tt 

2.33 

23.72 

8 

1.0587 

28 

.2365 

48 

1.4617 

ti 

0 

24.50 

9 

1.0661 

29 

.2464 

49 

.4742 

20 

0 

10.20 

10 

1.0734 

30 

.2568 

50 

.4867 

" 

5.60 

23.60 

11 

1.0814 

31 

1.2673 

51 

.5010 

u 

0 

25.70 

12 

1.0894 

32 

1.2778 

52 

.5153 

10 

0 

9.10 

13 

1.0974 

33 

1.2883 

53 

.5296 

u 

8.75 

8.00 

14 

.1054 

34 

1.2988 

54 

.5439 

it 

16.70 

16.65 

15 

.1134 

35 

1.3093 

55 

1.5582 

" 

13.80 

23.35 

16 

.1215 

36 

1.3199 

56 

1  .  5729 

0 

0 

8.25 

17 

.1297 

37 

1  .  3305 

57 

1  .  5876 

tt 

7.52 

6.51 

18 

.1378 

38 

1.3411 

58 

1.6023 

It 

13.37 

6.33 

18 
19 

.1378 
.  1458 

38 
39 

1.3411 
1.3517 

58 
59 

1.6023 
1.6170 

11 
It 

16.80 
18.45 

8.70 
10.23 

Fe2Cl6+12H2O 

20 

1542 

40 

1.3622 

60 

1.6317 

It 

20.40 

15.40 

11 

20  10 

16  00 

(Franz,  J.  pr.  (2)  5.  283.) 

It 

19.95 

17.70 

Sp.  gr.  of  Fe2Cl6+Aq  at  17.5°. 

It 
It 

19.00 
18.05 

22.75 
23.40 

<y 

O7< 

—10 

0 

7.40 

FeTfcle 

Sp.  gr. 

Fe^Cle 

Sp.  gr 

Fe2Cl6 

Sp.  gr. 

tt 

19.46 

10.37 

tl 

20.48 

20.54 

1 

1.008 

21 

1.191 

41 

1.428 

(I 

20.25 

21.56 

2 

1.016 

22. 

.202 

42 

1.441 

—12.5 

22.14 

16.69 

3 

1.025 

23 

.212 

43 

1.454 

—15 

0 

6.98 

4 

1.033 

24 

.223 

44 

1.469 

a 

21.30 

9.65 

5 

1.042 

25 

.234 

45 

1.481 

—20 

0 

6.56 

6 

1.051 

26 

.245 

46 

1.494 

tt 

7.50 

4.90 

7 

1.060 

27 

.256 

47 

1.507 

" 

15.30 

5.09 

8 

1.069 

28 

.268 

48 

1.520 

it 

20.56 

7.08 

9 

1.078 

29 

.280 

49 

1.533 

30 

o 

25.20 

10 

1.087 

30 

.292 

50 

1.547 

4.25 

27.80 

11 

1.095 

31 

.304 

51 

1.560 

tt 

o 

30.24 

12 

1.104 

32 

.316 

52 

1.573 

25 

o 

23.50 

13 

1.113 

33 

.328 

53 

1.587 

tt 

2.33 

23.72 

14 

1.123 

34 

.340 

54 

1.600 

11 

7.50 

29.75 

15 

1.131 

35 

.352 

55 

1.612 

ti 

0 

31.50 

16 

1.140 

36 

1.364 

56 

1.624 

20 

o 

22.50 

17 

1.150 

37 

1.376 

57 

1.636 

5.60 

23.60 

18 
19 

1.160 
1.170 

38 
39 

1.390 
1.403 

58 
59 

1.648 
1.659 

ti 

n 

ii!os 

11  05 

29.20 
29.20 

Fe2C]6+7H2O 

20 

1.180 

40 

1.415 

60 

1.670 

it 

0 

32^00 

(Hager,  Comm.  1883.) 

15 
ti 

10.75 
14.90 

23.50 
28.35 

Sp.  gr.  of  cone.  Fe2Cl6+Aq  at  20-21°. 

10 

13.80 
17  sn 

23.35 

A 

Sp.  gr. 

Fe2CI< 

Sp.  gr. 

Fe'2Cl6 

Sp.  gr. 

it 

0 

1  1  .  oU 

17.80 
18.05 

27  '.75 
23.40 

60 

1.669 

65 

715 

70 

1.758 

a 

19.50 

25.93 

61 

1.679 

66 

.724 

71 

1.766 

62 

1.688 

67 

.733 

72 

1.774 

63 

1.697 

68 

.742 

73 

1.782 

64 

1.706 

69 

.750 

74 

1.790 

(Hager,  1.  c.) 

IRON  CHLORIDE 


429 


Solubility  of  Fe2Cl6  in  HCl+Aq.  —  Continued. 

Sat.  solution  contains 

Sat.  solution  contains 
per  100  mols.H2O 

t 

per  100  mols.  H2O 

Solid  phase 

1 

t° 

Solid  phase 

mols.  HC1 

rnois. 
FeCls 

mols. 

mols.  HC1 

FeCls 

33 

30.45 

48.70 

50 

0 

35.00 

30 

17.15 

36.75 

(i 

3.25 

39.95 

(S 

31.20 

43.49 

44 

0 

33.50 

- 

fC 

33.80 

47.80 

ii 

3.04 

33.80 

<c 

32.60 

49.93 

(i 

10.62 

34.64 

25 

19.50 

35.25 

ii 

11.50 

35.60 

44. 

20.60 

35.34 

ii 

10.70 

38.00 

44 

31.34 

41.58 

40 

0 

32.40 

44 

33.00 

43.00 

it 

13.40 

37.45 

44 

34.65 

44.80 

33 

0 

31.00 

20 

21.25 

34.25 

ii 
30 

15.70 
0 

37.06 
30.24 

44 

11 

28.81 
34.23 

37.57 
42.02 

Fe2Cl6+4H2O 

u 

17.20 

34.00 

(I 

35.40 

43.16 

u 

17.15 

36.75 

15 

29.40 

36.50 

25 

0 

29.00 

u 

33.60 

40.03 

« 

7.50 

29.75 

Fe2Cl6+5H2O 

10 

24.50 

32.75 

a 

19.50 

35.25 

" 

35.04 

39.95 

20 

0 

27.90 

0 

26.00 

32.16 

ti 

11.05 

29.20 

" 

34.60 

38.11 

a 

15.80 

30.68 

—10 

27.30 

32.05 

u 

21.25 

34.25 

H 

33.56 

36.25 

15 

14.90 

28.35 

*  :  "  ; 

—20 

30.08 

32.76 

u 

16.40 

29.32 

44 

32.65 

35.44 

10 

17.80 

27.75 

45 

0 

.58.00 

K 

18.80 

28.70 

" 

31.28 

50.08 

t( 

24.50 

32.75 

(i 

40.65 

48.60 

0 

24.12 

30.04 

40 

0 

58.00 

a 

26.00 

32.16 

u 

27.00 

50.80 

—10 

24.95 

29.60 

u 

42.01 

48.64 

Fe2Cl6 

It 

26.05 

30.50 

35 

0 

58.00 

anhydrous 

11 

27.30 

32.05 

|| 

29.01 

50.33 

70 

0 

44.0 

\ 

(4 

37.04 

49.20 

« 

6.75 

50.00 

30 

0 

58.00 

a 

0 

55.80 

tt 

32.60 

49.93 

65 

0 

42.50 

{( 

34.40 

49.72 

u 

10.25 

50.00 

40 

42.50 

47  .  52 

<i 

3.75 

57.25 

44 

42.01 

48.64 

44 

0 

59.00 

35 

39.47 

46.57 

60 

0 

41.40 

44 

37.04 

49.20 

44 

14.25 

50.00 

30 

40.21 

42.54 

u 

10.70 

55.25 

44 

38.20 

44.70 

a 

0 

61.00 

44 

35.55 

47.30 

55 

0 

40.64 

(( 

34.40 

49.72 

« 

19.00 

50.72 

25 

40.41 

40.25 

u 

16.71 

53.60 

44 

39.03 

41.38 

(i 

0 

62.00 

Fe2Cl6+4H2O 

11 

35.74 

45.24 

50 

0 

39.92 

20 

39.50 

39.25 

Fe2Cl6,  2HC1, 

14 

3.25 

39.95 

44 

35.40 

43.16 

4H20 

(| 

21.24 

49.33 

10 

38.62 

37.48 

44 

20.04 

52.50 

(4 

37.46 

38.33 

44 

0 

39.00 

44 

36.30 

38.70 

(4 

10.70 

38.00 

(( 

35.04 

39.93 

14 

14.80 

38.70 

0 

37.27 

36.60 

a 

24.14 

50.10 

tt 

34.60 

38.11 

40 

13.40 

37.45 

—10 

37.92 

35.32 

44 

27.00 

50.80 

44 

34.54 

36.00 

33 

15.70 

37.06 

1C 

33.56 

36.25 

a 

29.20 

42.70 

—20 

37.80 

34.50 

(4 

31.08 

46.85 

(i 

34.10 

34.84 

a 

30.81 

47.65 

(t 

32.56 

35.44 

430 


IRON  CHLORIDE 


Solubility  of  Fe2Cl6  in  HCl+Aq.—  Continued. 

Solubility  of  FeCl3+KCl  in  H2O  at  21°. 

Substance  added 

Pts.  by  weight  sol.  in  100 
pts.  of  solution 

Sat.  solution  contains 

per  100  mols.  H2O 

-l° 

Solid  phase 

FeCls  grams 

KC1  grams 

FeCls 

KCl 

mols. 

mols.  HC1 

FeCls 

0~T 

0_ 

Q 

Q4  07 

—  4.5 

a 

it 
—  6 

u 
u 

20.50 
20.66 
23.42 
29.10 
26.18 
24.41 
23.25 
21.73 
19.73 

24.50 
25.74 
27.40 
24.73 
21.75 
21.50 
21.35 
21.84 
25.50 

13 
18 
3 
.      28 
31 
36.2 
41.5 
46.5 

28   . 
21 
18.5 
16 
10.5 
9 
8 
6 
0   ^ 

13.44 
23.18 
28.05 
35.72 
36.62 
37.35 
42.03 
51.69 

OTT  .  i7  4 

24.45 
16.54 
11.69 
11.68 
11.19 
13.67 
7.88 
7.54 

11 
(I 

24.42 
28.20 

28.45 
27.04 

155 

\J  .  O 

0 

83^89 

0 

—10 

it 

20.48 
24.90 

20.54 
18.94 

(Hinrichsen  and  Sachsel,  Z.  phys.  Ch.  1904, 
50.  95.) 

11 

28.75 

20.34 

11 

31.42 

28.25 

28.53 
30.25 

Fe2Cl6,  2HC1, 
8H20 

FeCl3+NaCl. 

15 

26.05 
24  50 

30.50 
15  83 

Solubility  of  FeCl3+NaCl  in  H2O  at  21°. 

—15 
—20 

28.40 
19.44 

31.89 
12.10 

Substance  added 

Pts.  by  weight  sol.  in  100 
pts.  of  solution 

" 

22.83 
25.20 

11.63 
11.60 

FeCls  grams 

NaCl  grams 

FeCls 

NaCl 

(( 

27.20 
31.08 
34.13 
33.93 
30.08 
28.70 

11.31 
11.51 
12.90 
31.77 
32.76 
32.88 

0 
1.8 
3.6 
5.5 

7.2 
9.0 

3.6 
3.0 
2.5 
2.0 
1.5 
1.0 

0 
24.27 
25.40 
26.40 
38.15 
43.38 

36.10 
9.10 

8.45 
5.25 
3.90 
2.45 

—10 

12.01 

11.99 

10.8 

0.5 

46.75 

2.11 

f* 

19.78 

14.02 

10.8 

0 

83.39 

0 

a 

20  95 

16.20 

« 

20.25 

20.20 

(Hinrichsen  and  Sachsel,  Z.  phys.  Ch.  1904, 

11 

17.73 

20.70 

50.  94.) 

11 

15.44 

19.65 

—12.5 

i  ^ 

22.14 

16.69 

9    ax 

Solubility  of  FeCl3  in  NaCl+Aq  at  t°. 

—  10 

tt 

—20 

tt 

24^50 
9.96 
13.32 

.  OO 

15.83 
9.94 

8.57 

Fe2Cl6,  2HC1, 
12H2O 

t° 

Substance  added 

%  of  Fe  in 
the  solution 

FeCls 

NaCl 

" 

16.90 

7.35 

10 

40 

20 

15.2 

it 
(( 

Jti 

a 

18.97 
20.56 
23.40 
•24.85 
25.20 
25.40 
25.59 

7.16 
7.08 
7.20 
9.88 
11.60 
12.37 
13.39 

10 
10 
20 
20 
20 
30 
30 

60 
100 
60 
80 
100 
70 
90 

20 
20 
20 
20 
20 
30 
30 

15.2 
15.16 
16.2 
16.18 
16.2 
17.7 
17.6 

30 

110 

30 

17.67 

(Roozeboom  and  Schreinemakers,   Z.  phys. 

50 

30 

20 

23.5 

Ch.  1894,  15.  633.) 

50 

45 

20 

23.9 

40 

35 

30 

25.4 

Solubility  of  Fe*Cl6+NH4Cl. 

40 

50 

30 

25.5 

See  NH4Cl+Fe2Cl6  under  NH4C1. 

30 

30 

20 

23.8 

30 

45 

20 

24.0 

Solubility  of  Fe2Cl6  in  CsCl. 

17.6 

30 

20 

24.47 

See  CsCl+Fe2Cl6  under  CsCl. 

17.6 

50 

20 

24.5 

(Hinrichsen  and  Sachsel,  Z.  phys.  Ch.  1904, 

50.95.) 

IRON  PHOSPHORIC  CHLORIDE 


431 


Difficultly  sol.  in  AsBr3.  (Walden,  Z. 
anorg.  1902,  29.  374.) 

Attacked  by  liquid  NO2  in  the  presence  of 
traces  of  moisture.  (Frankland,  Chem.  Soc. 
1901,  79.  1361.) 

Sol.  in  liquid  SO2.  (Walden,  B.  1899,  32. 
2864.) 

Sol.  in  alcohol  ether,  acetic  ether  (Cann, 
C.  R.  102.  363),  and  acetone  (Krug  and 
M'Elroy,  J.  anal.  Ch.  6.  184). 

SI.  sol.  in  ethylamine.  (Shinn,  J.  phys. 
Chem.  1907,  11.  538.) 

Sol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1369.) 

Sol.   in  methyl   acetate.      (Naumann,   B. 

1909,  42.  3790.) 

Insol.   in   ethyl   acetate.      (Naumann,    B. 

1910,  43.  314.) 

1  g.  FeCl3  is  sol.  in  1.59  g.  acetone  at  18°. 
Sp.  gr.  of  sat.  solution  18°/4°  =  1.160.  (Nau- 
mann, B.  1904,  37.  4333.) 

Sol.  in  acetone  and  in  methylal.  (Eidmann, 
C.  C.  1899,  II.  1014.) 

Sol.  in  quinoline.  (Beckmann  and  Gabel, 
Z.  anorg.  1906,  51.  236.) 

SI.  sol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.  257.) 

Mol.  weight  determined  in  pyridine. 
(Werner,  Z.  anorg.  1897,  15.  22.) 

Sublimed. 

Sol.  in  AsCl3,  POC13,  SO2C12  and  PBr3;  si. 
sol.  in  PC13.  (Walden,  Z.  anorg.  1900,  25. 
214.) 

The  salts  with  different  amts.  of  crystal 
H2O  have  different  solubilities.  (Roozeboom. 

+4H2O.    Melts  in  crystal  H2O  at  73.5°. 

100  mols.  H2O  dissolve  mols.  Fe2CU  from 
Fe2Cl6+4H2O  at  t°. 


t° 

Mols. 
Fe2Cls 

t° 

Mols 

Fe2Cl6 

21.53 
23.35 
25.00 

t° 

Mols. 
Fe2Cl6 

50 
55 
60 

19.96 
20.32 
20.70 

69 
72.5 
73.5 

72.5 
70 

66 

26.15 
27.90 
29.20 

(Roozeboom,  Z.  phys.  Ch.  10.  477.) 
+5H2O.    Correct  formula  for  +6H2O  salt. 

100  mols.  H2O  dissolve  mols.  Fe2Cl6  from 
Fe2Cl6+5H2O  at  t°. 


t° 

Mols. 
Fe2Cl6 

12.87 
13.95 
14.85 

t° 

Mols. 
FesCle 

15.12 
15.64 
17.50 

t° 

Mols. 
Fe2Cl6 

12 
20 
27 

30 
35 
50 

55 
56 
55 

19.15 
20.00 
20.32 

(Roozeboom.) 

Melts  in  crystal  H2O  at  31°  (Engel,  C.  R. 
104.  1708);  at  56°  (Roozeboom). 

+6H2O.  Very  deliquescent.  Sol.  in  al- 
cohol. .Ether  dissolves  out  Fe2Cl6. 


M.-pt.  is  31°.     (Ordway.)     Contains  only 
5H2O.    (Roozeboom.) 

+7H2O.    Melts  in  crystal  H2O  at  32.5°. 

100  mols.  H2O  dissolve  mols.  Fe2Cl6  from 
Fe2ClG+7H20  at  t°. 


t 

Mols. 
Fe2Cl6 

t° 

Mols. 
Fe2Cl6 

t° 

Mols. 
Fe2Cl6 

20 
27.4 

11.35 
12.15 

32 
32.5 

13.55 
14.99 

30 
25 

15.12 
15.54 

(Roozeboom.) 

+12H20.     Less  deliquescent  than  Fe2Cl6 
or  Fe2Cl6+5H2O. 

100  mols.  H2O  dissolve  mols.  Fe2Cl6  from 
Fe2Cl6  +  12H2Oatt°. 


t 

Mols. 
Fe2Cl6 

t° 

Mols. 
FejCk 

t° 

Mols. 
Fe2Cl6 

—55 
—41 

—27 
0 
10 

2.75 
2.81 
2.98 
4.13 
4.54 

30 
35 
36.5 
37 
36 

5.93 
6.78 
7.93 
8.33 
9.29 

27.4 
20 
10 

8 

11.20 
12.15 
12.83 
13.70 

20 

5.10 

30 

10.45 

(Roozeboom.) 

Sol.  in  alcohol.    Ether  dissolves  out  Fe2Cle. 
Melts  in  crystal  H2O  at  37°  (Roozeboom) ; 
at  35.5°  (Ordway). 

Ferric  hydrogen  chloride,  FeCl3,  HC1+2H2O. 

Decomp.  by  H2O.  (Sabatier,  Bull.  Soc.  (2) 
197.) 

More  sol.  in  H2O  than  FeCl3.  (Engel,  C.  R. 
104.  1708.) 

For  solubility,  see  FeCl8+HCl,  under 
ferric  chloride. 

+6H2O.  (Roozeboom  and  Schreinemak- 
ers.) 

For  solubility,  see  FeCl3+HCl,  under 
ferric  chloride. 

Ferrous  lithium  chloride,  FeCl2,  LiCl+3H2O. 
(Chassevant,  A.  ch.  (6)  30.  17.) 

Ferric  magnesium  chloride,  FeCl3,  MgCl2  + 

H2O. 
Deliquescent.    (Neumann,  B.  18.  2890.) 

Ferrous  mercuric  chloride,  FeCl2,  HgCl2  + 

4H2O. 
Deliquescent,    (v.  Bonsdorff.) 

Ferric  nitrosyl  chloride,  FeCl3,  NOC1. 

Very   deliquescent.      (Weber,    Pogg.    118. 

477.) 

Ferric  phosphoric  chloride,  FeCl3,  PC16. 

Decomp.  by  H2O.  (Baudrimont,  A.  ch.  (4) 
2.  15.) 


432 


IRON  POTASSIUM  SULPHIDE 


Iron    (ferrous)    potassium    chloride,    FeCl2, 

2KC1+2H2O. 
Sol.  in  H2O.    (Berzelius.) 

Ferric  potassium  chloride,  FeCl3,  2KC1+ 
H2O. 

A  little  H2O  dissolves  out  FeCl3 .  (Fritzsche 
J.  pr.  18.  483.) 

Sol.  in  H2O.  (Walden,  Z.  anorg.  1894,  71. 
332.) 

Ferric  rubidium  chloride,  FeCl3,  3RbCl. 

Easily  sol.  in  H2O.  Insol.  in  HCl+Aq. 
(Godeffroy,  Arch.  Pharm.  (3)  9.  343.) 

FeCl3,  2RbCl+H2O.  Decomp.  by  H2O. 
(Neumann,  A.  244.  329.) 

Sol.  in  H2O.  (Walden,  Z.  anorg.  1894,  7. 
332.) 

Ferric  sulphur  chloride,  FeCl3,  SC14. 

Very  sensitive  toward  heat  and  moisture. 
(Ruff,  B.  1904,  37.  4518.) 

Ferric  thallium  chloride,  FeCl3,  3T1C1. 

Decomp.  by  H<>O.  Can  be  crystallised  from 
HCl+Aq.  (Wohler,  A.  144.  250.) 

Ferrous  chloride  ammonia,  3FeCl2,  2NH3. 

Decomp.  by  H2O.  (Rogstadius,  J.  pr.  86. 
310.) 

FeCl2,6NH3.  Loses  4NH3  at  100°.  (Miller, 
Am.  Ch.  J.  1895,  17.  577.) 

FeCl2,  2NH3.    Decomp.  in  the  air  (Miller). 

Ferric  chloride  ammonia,  FeCl3,  NH3. 

Slowly  deliquescent.  Sol.  in  H2O  with 
evolution  of  heat.  (Rose,  Pogg,  24.  302.) 

FeCl3,  6NH3.  Not  deliquescent;  not  sol. 
in  H2O;  sol.  in  HC1  with  decomp.  (Miller, 
Am.  Ch.  J.  1895,  17.  577.) 

Loses  NH3  to  give  FeCl3,  5NH3,  and  FeCl3, 
4NH3. 

Ferric  chloride  cyanhydric  acid,  FeCl3, 2HCN. 
Deliquescent.    (Klein,  A.  74.  85.) 

Ferrous  chloride  nitric  oxide,  FeCl2,  NO. 

Sol.  in  H2O  without  evolution  of  gas. 
(Thomas,  C.  R.  1895,  121.  204.) 

+2H2O.  Sol.  in  cold  H2O  without  decomp. 
(Thomas,  C.  R.  1895,  120.  448.) 

2FeCl2,  NO.  Very  hydroscopic.  (Thomas, 
C.  R.  1895,  121.  129.) 

10FeCl2,  NO.  Very  hygroscopic.  (Thomas 
C.  R.  1895,  121.  128.) 

Ferric  chloride  nitric  oxide,  Fe2Cl6,  NO. 

Very  hygroscopic.  Loses  NO  when  ex- 
posed to  the  air. 

2Fe2Cl6,  NO.  Very  hygroscopic.  In  con- 
tact with  H2O  gives  off  NO.  (Thomas,  C.  R. 
1895,  120.  447.) 


Iron  (ferrous)  fluoride,  FeF2.    » 

SI.  sol.  in  H2O;  insol.  in  alcohol  and  ether. 
Partly  sol.  in  hot  HCl+Aq;  slowly  sol.  in 
cold,  easily  in  hot  HNO3;  decomp.  by  H2SO4. 
(Poulenc,  C.  R.  115.  941.) 

+8H2O.  Difficultly  sol.  in  H2O;  more 
easily  if  it  contains  HF.  (Berzelius.) 

Ferroferric  fluoride,  FeF3,  FeF2-f  7H2O. 

Sol.  in  dil.  HF+Aq.  (Weinland,  Z.  anorg. 
1899,  22.  268.) 

Ferric  fluoride,  FeF3. 

SI.  sol.  in  H2O;  insol.  in  alcohol  or  ether. 
SI.  attacked  by  HNO3,  HC1,  or  H2SO4+Aq. 
(Poulenc,  C.  R.  115.  941.) 

+4^H^O.  More  sol.  in  hot  than  cold  H2O. 
Insol.  in  alcohol.  (Scheurer-Kestner,  A.  ch. 
(3)  68.  472.) 

Ferric  nickel  fluoride,  FeF3,  NiF2+7H2O. 

SI.  sol.  in  dil.  HF+Aq.  (Weinland,  Z. 
anorg.  1899,  22.  268.) 

Ferrous  potassium  fluoride,  FeF2,  KF+2H2O. 
(Wagner,  B.  19.  896.) 
FeF2,2KF.    SI.  sol.  in  H2O.    (Berzelius.) 

Ferric  potassium  fluoride,  FeF3,  2KF. 

Somewhat  sol.  in  H2O,  especially  if  hot. 
(Berzelius.) 

+H2O.    (Christensen,  J.  pr.  (2)  35.  164.) 
FeF3,  3KF.     Properties  as  above.     (Ber- 
zelius.) 

Ferric  sodium  fluoride,  FeF3,  2NaF+3^H2O. 

Rather  easily  sol.  in  H2O.  Solution  de- 
comp. on  heating.  Very  sol.  in  FeCl3+Aq. 
(Nickles,  J.  Pharm.  (4)  10.  14.) 

FeF3,  3NaF.    (Wagner,  B.  19.  896.) 

Ferric  thallous  fluoride,  2FeF3,  3T1F. 

Sol.  in  hot  H2O,  less  sol.  in  cold.  SI. 
sol.  in  HF.  (Ephraim,  Z.  anorg.  1909,  61. 
239.) 

Ferrous  titanium  fluoride. 
See  Fluotitanate,  ferrous. 

Ferric  zinc  fluoride,  FeF3,  ZnF2+7H2O. 

SI.  sol.  in  dil.  HF+Aq.  (Weinland,  Z. 
anorg.  1899,  22.  269.) 

Ferrous  hydroxide,  FeO2H2. 

Sol.  in  150,000  pts.  H2O.  (Bineau,  C.  R. 
41.  509.) 

Insol.  in  KOH,  or  NaOH+Aq.  Sol.  in 
NH4  salts +Aq.  SI.  sol.  in  NaC2H3O2+Aq. 
(Mercer.) 

Not  pptd.  in  presence  of  Na  citrate.  Insol. 
in  boiling  cane  sugar +Aq,  but  si.  sol.  when 
KOH  has  been  added.  Not  pptd.  in  presence 
of  much  H2C4H4O6.  (Rose.) 


IRON  HYDROXIDES 


433 


Solubility  in  glycerine -j-Aq  containing 
about  60%  by  vol.  of  glycerine. 

100  ccm.  of  the  solution  contain  1.0  g.  FeO 
(Muller,  Z.  anorg.  1905,  43.  322.) 

Iron  (ferric)  hydroxides,  Fe2O3,  rcH2O. 

Many  indefinite  compounds  of  Fe2O3  and 
H2O  are  known,  and  uncertainty  exists  as  to 
their  composition. 

According  to  van  Bemmelen  (R.  t.  c.  7. 106) 
there  are  probably  no  true  definite  compounds 
of  Fe2O3  and  H2O. 

According  to  Tommasi  (B.  12.  1924,  2334), 
there  are  two  series  of  Fe  hydroxides,  a,  red 
hydroxides,  and  /3,  yellow  hydroxides. 

a  Hydroxides.  Fe2O6H6  (unstable),  Fe2O3, 
2H2O  (loses  H2O  at  50°),  and  Fe2O3,  H2O  (loses 
H20  at  92°). 

Sol.  in  dil.  acids  and  in  Fe2Cl6+Aq,  and 
pptd.  from  the  latter  solution  by  Na2SO4,  or 
H2S04+Aq. 

j3  Hydroxides.  Fe2O6H6  (stable  below  70°), 
Fe2O3,  2H2O  (loses  H2O  at  105°),  Fe2O3,  H2O 
(loses  H2O  at  150°). 

SI.  sol.  in  acids,  and  insol.  in  Fe2Cl6+Aq. 
(Tommasi.) 

The  following  more  or  less  uncertain  data 
are  given. 

2Fe2O3,  H2O.  Sol.  in  HCl+Aq.  Very  si. 
sol.  in  HNO3+Aq.  (Davies,  Chem.  Soc. 
(2)  4.  69.) 

Min.  Turgite. 

Fe2O3,*H2O.  Insol.  in  cold  acids,  difficultly 
sol.  in  warm  HC1  and  H2SO4+Aq,  and  especi- 
ally in  warm  HNO3+Aq.  (Schiff,  A.  114. 199.) 

Min.  Gothite. 

2Fe2O3,  3H2O.  SI.  sol.  in  tartaric,  citric, 
or  acetic  acids,  but  easily  sol.  in  HCl+Aq. 
(Wittstein.) 

Scarcely  attacked  by  cone.  HNO3,  or  HC1+ 
Aq.  Sol.  in  acetic  acid  or  dil.  HNO3,  or  HC1  + 
Aq,  from  which  solution  it  is  pptd.  by  trace  of 
alkali  salts.  (St.  Gilles.) 

Min.  L-imonite. 

3Fe2O3,  5H2O.    (Muck.) 

Fe2O3,  2H2O.    Easily  sol.  in  HCl+Aq. 

Min.  Xanthosiderite. 

Fe2O3,  3H2O.  SI.  sol.  in  acetic  acid  of  1.03 
sp.  gr.,  but  easily  sol.  if  of  1.076  sp.  gr.  Sol. 
in  mineral  acids.  (Limberger,  J.  B.  1863.  70.) 

Pptd.  Fe2O3,  xH2O=Fe2O6H6(?).  Insol. 
in  H2O,  or  in  solutions  of  the  alkalies  or  NH4 
salts.  When  recently  pptd.  is  easily  sol.  in 
acids.  (Fresenius.) 

SI.  sol.  in  NH4OH,  and  NH4  salts +Aq. 
(Odling.) 

Apparently  insol.  in  NH4C1,  or  (NH4)2CO3 
+Aq.  (Brett,  1837.) 

SI.  sol.  in  cone.,  but  insol.  in  dil.  KOH+Aq. 
(Chodnew,  J.  pr.  28.  221.) 

SI.  sol.  in  very  cone.  KOH+Aq  free  from 
CO2.  (Volcker,  A.  69.  34.) 

Not  at  all  sol.  in  pure  cone.  KOH+Aq, 
solubility  noticed  by  previous  observers  being 
caused  by  the  presence  of  silicic  acid.  (Sand- 
rock.) 


SI.  sol.  in  cone,  alkali  carbonates +Aq. 

When  freshly  pptd.,  it  is  not  acted  upon  by 
cone.  K2CO3+Aq.  (Grotthaus.) 

Readily  sol.  in  cone.  (NH4)2CO3+Aq,  but 
pptd.  by  addition  of  H2O. 

Sol.  in  excess  of  (NH4)2CO3+Aq  when 
pptd.  by  that  reagent.  (Wohler.) 

Sol.  in  solutions  of  the  alkali  bicarbonates. 
(Berzelius.) 

Sol.  in  aqueous  solutions  of  water-glass. 
(Ordway.) 

Immediately  dissolved  by  H2SO3+Aq. 

Sol.  in  NH4F+Aq.     (Helmholt,  Z.  anorg. 

Sol.  in  cone.  Al2(SO4)3+Aq.  (Schneider, 
B.  23.  1352:) 

SI.  sol.  in  a  solution  of  MgCO3(?).  (Bis- 
chof). 

Insol.  in  ethylamine,  or  amylamine+Aq. 
(Wurtz,  A.  ch.  (3)  30.  472.) 

Sol.  in  boiling  solution  of  Bi(NO3)3,  with 
pptn.  of  Bi2O3.  (Persoz.) 

Sol.  in  Cr2Cl6+Aq;  after  3  months  15  mols. 
Fe2O6H6  were  dissolved  by  1  mol.  Cr2Cl6. 
(Bechamp,  A.  ch.  (3)  57.  296.) 

Insol.  in  fumaric  acid,  even  when  freshly 
pptd. 

When  recently  pptd.,  it  is  easily  sol.  in 
KHC4H4O6+Aq,  but  after  drying  it  is  dif- 
ficultly sol.  therein. 

When  moist  easily  sol.  in  H2C4H4O6+Aq, 
but  after  drying  is  scarcely  sol.  therein  when 
cold,  and  only  si.  sol.  when  hot.  (Werther.) 

Easily  sol.  in  acetic,  citric,  and  other  acids. 
(Wittstein.) 

Solubility  in  glycerine +Aq  containing 
about  60%  by  vol.  of  glycerine. 

100  ccm.  of  the  solution  contain  0.8  g. 
Fe2O3.  (Muller,  Z.  anorg.  1905,  43.  322.) 

Easily  sol.  in  aqueous  solution  of  su crates 
of  Ca,  Ba,  Sr,  K,  Na.  (Hunton,  1837.) 

Unacted  upon  by  cane  sugar +Aq.  (Glad- 
stone*) 

SI.  sol.  in  cane  sugar +Aq,  from  which  it  is 
pptd.  by  (NH4)2S+Aq,  but  not  by  NH4OH, 
or  K4FeC6N6+Aq.  (Peschier.) 

Solubility  of  Fe2O6H6  in  sugar  solutions.  1  1. 
of  sugar  solution  of  given  strength  dis- 
solves mg.  of  Fe2OeH6. 


Mg.  Fe2O6H6 

%  Sugar 

at  17.4° 

at  45° 

at  75° 

10 

3.4 

3.4 

6.1 

30 

2.3 

2.7 

3.8 

50 

2.3 

1.9 

3.4 

fStolle,  Z.  Ver.  Zuckerind.  1900,  60.  340.) 

Not  pptd.  from  solutions  by  alkalies  or 
alkali  carbonates  in  presence  of  many  organic 
substances,  as  tartaric  acid,  sugar,  etc.  \ 

Not  pptd.  by  NH4OH  from  solutions  con- 
taining Na4P2O7.  (Rose,  Pogg.  76.  19.) 

Not  pptd.  by  NH4OH  in  presence  of  Na 
citrate.  (Spiller.) 


434 


IRON  HYDROXIDE 


Soluble,  (a)  By  dialysis.  Solutions  con- 
taining 1%  can  be  concentrated  somewhat 
whereupon  they  gelatinise.  They  also  gela- 
tinise by  cold,  or  addition  of  traces  of  H2SO4, 
alkalies,  alkali  carbonates  or  sulphates,  or 
neutral  salts,  not,  however,  by  HC1,  HN03 
alcohol,  or  sugar.  (Graham,  A.  121.  46.) 

When  a  dil.  solution  of  a  solid  organic  acid 
or  an  alkali,  or  salt  is  added  to  a  dialysed 
solution  of  Fe2O6H6,  a  coagulum  sol.  in  H2O 
is  formed,  but  if  the  solutions  are  cone,  the 
separating  coagulum  is  no  longer  sol.  in  HoO 
(Athenstadt,  C.  C.  1871.  822.) 

(6)  Pean  St.  Gilles'  hydroxide,  or  meta-iron 
hydroxide.  Sol.  in  H2O.  Pptd.  from  solution 
by  traces  of  H2SO4,  HC1,  HNO3+Aq,  and 
alkalies;  the  ppt.  is  insol.  in  cold  acids,  but 
sol.  in  pure  H2O.  (Pean  St.  Gilles,  A.  ch.  (3) 
46.  47.) 

See  also  table  by  Krecke  in  the  article  on 
ferric  chloride. 

Iron  (Ferroferric)  hydroxide,  Fe3O4,  H2O  (?). 
Sol.  in  acids. 
Fe3O4,  4H2O.    (Lefort.) 

Ferrous  iodide,  FeI2. 

Very  deliquescent.  Sol.  in  H2O.  Solution 
decomp.  on  evaporating.  ' 

4-4H2O.  Very  deliquescent;  si.  sol.  in 
H2O;  sol.  in  ether.  (Jackson,  Am.  Ch.  J. 
1900,  24.  19.) 

-f-5H2O.  Deliquescent.  Sol.  in  alcohol. 
Sol.  in  sugar +Aq,  and  solution  is  much  -more 
stable  than  aqueous  solution.  Easily  sol.  in 
glycerine. 

Insol.  in  methylene  iodide.  (Retgers,  Z. 
anorg.  3.  343.) 

+6H2O,  and  +9H2O.  Very  sol. ;  pptd.  from 
cooled  aq.  solution.  (Volkmann,  C.  C.  1894, 
II.  611.) 

Ferric  iodide,  FeI3. 

Has  not  been  isolated.  Solution  of  I  in 
FeI2+Aq  in  the  molecular  ratio  of  I  :  FeI2 
probably  contains  FeI3. 

Very  sol.  in  liquid  NH3.  (Franklin,  Am. 
Ch.  J.  1898,  20.  828.) 

Ferrous  mercuric  iodide,  FeI2,  2HgI2+6H2O. 
As  the  corresponding  Mg  salt.     (Duboin, 
C.  R.  1907,  145.  714.) 

Ferrous  iodide  ammonia,  FeI2,  6NH3. 

Decomp.  by  H2O.  (Jackson,  Am.  Ch.  J. 
1900,  24.  27.) 

Ferrous  mercuric  iodide. 

Very  deliquescent.  Decomp.  by  H2O;  sol. 
in  HC2H3O2  or  alcohol. 

Iron  molybdenide,  FeMo2. 

Attacked  by  HCl+Aq  with  difficultly 
Sol.  in  hot  cone.  H2SO4.  (Steinacker.) 


Iron  nitride. 

Easily  decomp.  by  H2O  when  finely  pow- 
dered. (Rossel,  C.  R.  1895,  121.  942.) 

Fe2N.  Easily  sol.  in  HNO3,  HC1,  or  H2SO4 
+Aq.  Very  slowly  decomp.  by  H2O.  (Stahl- 
schmidt,  Pogg.  125.  37.)  . 

Sol.  in  HC1  with  decomp.;  decomp.  by 
steam  and  by  H2S  at  200°.  (Fowler,  C.  N. 
1894,  68.  152.) 

FesNa.  Probably  the  same  as  the  above 
compound.  (Rogstadius,  J.  pr.  86.  307.) 

Iron  nitrososulphantimonate,  Fe4S(NO)6Sb2S5. 

(Low,  C.  C.  1865.  948.) 

Does  not  exist,  but  was  impure  sodium  fer- 
rofefranitrososulphide.  (Pawel,  B.  15.  2600.) 

Iron  nitrososulphides. 

See  Ferrofefranitrososulphydric  acid  and 
Ferro/ieptanitrososulphide,  ammonium. 

Fe3S5H2(NO)4.    (Roussin,  C.  R.  46.  224.) 

Fe3S3(NO)4+2H2O.  (Porczinsky,  A.  125. 
302.) 

Fe6S5(NO)19+4H2O.  (Rosenberg,  B.  3. 
312.) 

The  compound  to  which  the  above  formula 
were  given  was  impure,  according  to  Pawel  (B. 
12.  1407  and  1949;  15.  2600),  and  contained 
more  or  less  Na  or  NH4.  Pawel  considers  the 
substance  as  NH4  salt  of  ferroAeptanitroso- 
sulphydric  acid,  which  see. 

Fe3S2N5O6  +  13^H2O.  Sol.  in  H2O,  alcohol, 
ether,  CHC13,  acetone  and  ethyl  acetate. 
Insol.  in  benzene  and  light  petroleum.  (Marie, 
C.  R.  1896,  122.  138.) 

Iron  sodium  nitrososulphide,  3Na2S,  Fe2S3, 
2NO. 

(Roussin.) 

Na8Fe8S9(NO)18.    (Rosenberg.) 
Correct  formula  is  Na2S2(NO)4Fe2,  sodium 
ferrotetfranitrososulphide. 

Iron  nitrososulphocarbonate,  Fe4S(NO)6CS2  + 
3H2O. 

(Low,  C..C.  1865.  948.) 

Correct  formula  is  NaS3(NO)7Fe4+2H2O, 
sodium  ferro/ieptanitrososulphide.  (Pawel, 
B.  15.  2600.) 

Ferrous  oxide,  FeO. 

Insol.  in  H2O.    Sol.  in  acids. 

Easily  sol.  in  HC1,  and  HNO3+Aq;  nearly 
insol.  in  H2SO4.  even  when  heated.  (Tissan- 
dier,  C.  R.  74.  531.) 

Ferric  oxide,  Fe2O3. 

Attacked  by  acids  with  difficulty,  the  more 
so  the  higher  it  has  been  heated.  HCl+Aq 
is  the  best  solvent,  in  which  it  is  more  quickly 
sol.  by  long  digestion  at  a  gentle  heat  than 

'  boiling.    (Fresenius.) 

Most  easily  sol.  in  16  pts.  of  a  mixture  of 
8  pts.  H2SO4  and  3  pts.  H2O.  (Mitscherlich, 
J.  pr.  81.  110.) 


IRON  OXIDE 


435 


Solubility  of  Fe2O3  in  HF+Aq  at  25°. 

Absolutely  insol.  in  Br2+Aq.    (Balard.) 
Insol.  in  hot  NH4Cl+Aq.    (Rose.) 
Insol.  in  KOH+Aq.    (Chodnew,  J.  pr.  28. 
222.) 
Slowly  sol.  in  an  aq.  solution  of  calcium 
hydrogen   carbonate.      The   velocity   of   the 
reaction  may  be  much  increased  by  the  addi- 
tion of  small  amounts  of  alkali  sulphate  or 
CaSO4.    (Rohland,  Z.  anal.  1909,  48.  629.) 
Insol.  in  benzonitrile.    (Naumann,  B.  1914, 
47.  1370.) 
Insol.  in  acetone.     (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 
Solubility  in  (calcium  sucrate+  sugar)  +Aq. 
1  1.  solution  containing  418.6  g.  sugar  and 
34.3  g.  CaO  dissolves  6.26  g.  Fe2O3;  296.5  g. 
sugar  and  24.2  g.  CaO  dissolves  4.71  g.  Fe2O3; 
174.4  g.  sugar  and  14.1  g.  CaO  dissolves  3.08  g. 
Fe2O3.    (Bodenbender,  J.  B.  1865.  600.) 

Solubility  of  Fe2O3  in  sugar  solutions.     1  1. 
of  sugar  solution  of  given  strength  dis- 
solves mg.  Fe2O3. 

Time 

G.  Fe2O3  in 
10  ccm.  of 
the  solution 

N-HF 

4^  hrs. 
21fc     " 
45^    " 

0.1581 
0.2235 
0.2279 

0.5N-HF 

2H    " 
8M    " 
23^    " 
56^    " 

0.0579 
0.0884 
0.1045 
0.1162 

0.25N-HF 

2M    " 
8^    " 
24%    " 
142^    " 

0.0180 
0.0345 
0.0475 
0.0534 

equal  amts. 
N-HF+N-HC1 

2M    " 
8^    " 
23M    " 
96 
264 

0.1011 
0.1611 
0.1976 
0.2223 
0.2297 

mg.  Fe2O3 

(Deussen,  Z.  anorg.  1905,  44.  414.)  ' 
Solubility  of  Fe2O3  in  HCl+Aq  at  25°. 

at  17.5° 

at  45° 

10                       1.4 
30                       1.4 

50                      0.8 

2.0 

i.i 

Time 

G.  ~FezOs  in 
10  ccm.  of 
the  solution 

(Stolle,  Z.  Ver.  Zuckerind,  1900,  60.  340.) 

Calcined. 
Solubility  of  calcined  Fe2O3  in  acids  at  25°. 

N-HC1 

4%  hrs. 
213^    " 
45^    " 

0.0409 
0.1230 
0.2125 

0.5N-HC1 

2%    " 
8^    " 
23^    " 
5Q1A    " 

0.0126 
0.0188 
0.0382 
0.0672 

Acid                         Time 

g.  Fe2Os  in 
10  ccm.  of  the 
solution 

N-HF                 4^  hrs. 
43^    " 
129K    " 

0.0889 
0.2035 
0.2194 

0.25N-HC1 

2X    " 
&A    " 
24%    " 
U21A    " 

0.0040 
0.0054 
0.0120 
0.0306 

N-HC1               4^    " 

43^    " 
1393/S    " 

0.0224 
0.1000 
0.1910 

equal  vol. 
N-HCl+N-NaF 

2%    " 

m  " 

23%    "     ' 
72^    " 
215 

0.0444 
0.0640 
0.0743 
0.0757 
0.0766 

(Deussen,  Z.  anorg.  1905,  44.  413.) 

See  also  Ferric  hydroxide. 
Min.  Hematite.     Rather  easily  sol.  in  HC1 
+Aq,  but  not  readily  sol.  in  other  acids. 

Metairon  oxide. 
See  Ferric  hydroxides. 

Ferroferric  oxide,  6FeO,  Fe2O3. 
FeO,  Fe2O3  =  Fe3O4.    With  insufficient  HC1 
+Aq  for  complete  solution,  FeO  is  dissolved 
and  Fe2O3  left.    (Berzelius.) 
Insol.  in  HNO3+Aq  at  the  ordinary  tem- 
perature.   (Millon.) 
Insol.  in  acetone.    (Naumann,  B.  1904,  37. 
4329.) 

(Deussen,  1.  c.) 
Solubility  of  Fe2O3  in  N-oxalic  acid  at  25°. 

rr,-                               G.  Fe2Os  in  10  ccm.  of 
'  Time                                    the  solution 

1%  hrs.                       0.0310 
6%    «                         0.0790 
22    "                         0.1960 
94    "                         0.2326 

(Deussen.) 

436 


IRON  OXIDE  ZINC  OXIDE 


Solubility  of  Fe2O4  in  sugar  solutions.  1  1.  of 
sugar  solution  of  given  strength  dissolves 
mg.  Fe?O4. 


mg.  FeaCU 

c/  Suear 

at  17.5° 

at  45° 

at  75° 

10 

10.3 

10.3 

12.4 

30 

12.4 

10.3 

12.4 

50 

14.5 

10.3 

14.5 

(Stolle,  Z.  Ver.  Zuckerind.  1900,  50.  340.) 

Min.  Magnetite.  Insol.  in  HNO3,  but  sol. 
in  hot  HCl+Aq. 

Iron  sesquioxide  zinc  oxide,  Fe2O3,  ZnO. 
See  Ferrite,  zinc. 

Ferric  oxybromide. 

Basic  ferric  bromides  containing  three 
equivalents,  or  less,  of  base  to  one  of  acid 
may  be  obtained  dissolved  in  H2O.  (Ordway, 
Am.  J.  Sci.  (2)  26.  202.) 

The  most  basic  soluble  compound  obtained 
by  three  months'  digestion  of  Fe2OeH6  with 
Fe2Br6+Aq,  is  Fe2Br6,  14Fe2O3.  (Bechamp.) 

Ferric  oxychlorides. 

(a)  Soluble.  Fe2O6H6  dissolves  in  Fe?Cl6  + 
Aq.  By  digesting  until  the  acid  reaction  of 
the  chloride  has  disappeared  a  solution  of 
Fe2Cl6,  2Fe2O3  is  obtained.  (Pettenkofer, 
Repert.  (2)  41.  289.) 

By  digesting  for  several  days  in  the  cold, 
Fe2Cl6,5Fe2O3  is  obtained,  and  still  more  basic 
compounds  by  further  addition  of  Fe2O6H6. 
When  the  solution  contains  Fe2Cl6,  12Fe2O3  it 
gelatinises,  but  still  dissolves  completely  in 
H2O.  The  most  basic  soluble  compound  is 
Fe2Cl6,  20Fe2O3.  (Bechamp,  A.  ch.  (3)  57. 
296.) 

If  the  digestion  is  carried  on  several  weeks, 
a  solution  containing  Fe2Cle,  23Fe2O3  is  ob- 
tained; this  can  be  boiled  and  diluted  with- 
out pptn.,  but  Fe2O6H6  is  precipitated  by  the 
addition  of  very  many  salts.  (Ordway,  Sill. 
Am.  J.  (2)  26.  197.) 

Solutions  containing  10  or  less  molecules 
Fe2O3  to  1  mol.  Fe2Cl6  can  be  dried  without 
the  oxychloride  becoming  insoluble.  (Ord- 
way.) 

The  above  solutions  do  not  become  cloudy 
by  boiling  or  diluting.  (Phillips.) 

A  very  dil.  solution  of  Fe2Cl6,  10Fe2O3  re- 
mains clear  after  protracted  boiling,  and  may 
be  boiled  without  decomp.  even  when  Fe2Cl6, 
20Fe2O3  is  present.  (Be" champ.) 

HNO3,  and  HCl+Aq  form  precipitates  in 
the  above  solutions,  which  are  sol.  on  addition 
of  more  H2O.  H2SO4+Aq  forms  a  precipi- 
tate insol.  in  H2O.  (Be"champ.) 

Fe2Cl6,  9Fe2O3  is  easily  sol.  in  H2O,  weak 
alcohol,  and  glycerine;  but  solutions  are  pptd. 
by  small  amts.  of  H2SO4,  M2SO4,  citric  or 


tartaric  acids,  or  a  few  drops  of  HC1,  or 
HNOa+Aq.  (Jeannel,  C.  R.  46.  799.) 

Solutions  containing  5  mpls.  Fe2O3  to  1  mol. 
Fe2Cl6  are  completely  precipitated  by  K2SO4, 
Na2S04,  MgS04,  KN03,  NaNO3,  Zn(NO3)2, 
KC1,  NaCl,  NH4C1,  CaCl2,  MgCl2,  ZnCl2, 
KBr,  or  KSCN.  (Bechamp.) 

Ba(NO3)2  does  not  precipitate  solutions  of 
less  than  18-20  Fe2O3  to  1  Fe2Cl6. 

Pb(NO3)2  or  Pb(C2H3O2)2  do  not  precipi- 
tate solutions  containing  the  compound 
Fe2Cle,  12Fe2O3,  but  a  mixture  of  the  two 
salts  causes  complete  precipitation. 

Solution  has-been  obtained  containing  116 
Fe2O3  to  1  FeCl6,  probably  owing  to  a  forma- 
tion of  soluble  colloidal  Fe2O3.  (Magnier  de 
la  Source,  C.  R.  90.  1352.) 

Solubility  determinations  in  the  system 
Fe2O3,  HC1  and  H2O,  show  that  at  25°  no 
definite  basic  chloride  is  formed,  but  that  the 
stable  solid  phase  is  one  of  a  series  of  solid 
solutions  containing  Fe2O3,  HC1  and  H2O. 
(Cameron,  J.  phys.  Chem.  1907,  11.  694.) 

(/3)  Insoluble.    Fe2Cl6,  6Fe2O3+9H2O. 

(1)  By  exposing  FeCl2+Aq  to  air.    Insol. 
in  H2O ;  si.  sol.  in  HCl+Aq.    (Wittstein.) 

(2)  From  FeCl2+Aq  and  HNO3.     Insol. 
in  H2O,  and  si.  sol.  in  HCl+Aq.    (Bechamp.) 

2Fe2Cl6,  25Fe2O3+41H2O.  Insol.  in  H2O. 
(Bechamp.) 

Fe2Cl6,  2Fe2O3+3H2O.  Decomp.  by  H2O 
with  residue  of  Fe2O3;  si.  sol.  in  dil.  acids. 
(Rousseau,  C.  R.  110.  1032.) 

Fe2Cl6,  3Fe2O3.  As  above.  (Rousseau, 
C.  R.  113.  542.) 

Ferric  oxyfluoride,  3Fe2O3,  2FeF3+4H2O. 
Ppt.    (Scheurer-Kestner.) 

Ferric  oxy sulphide,  Fe2O3,  3Fe2S3. 
(Rammelsberg.) 

Iron  phosphide,  FeP. 

Very  slowly  (Freese),  not  (Hvoslef,  A.  100. 
99)  sol.  in  hot  HCl+Aq.  Still  more  insol.  in 
dil.  H2SO4+Aq.  (Freese.) 

Slowly  sol.  in  HNO3+Aq,  and  easily  sol. 
in  aqua  regia.  (Struve.) 

Insol.  in  ammonum  citrate +Aq;  si.  sol. 
in  HC1.  (Dennis,  J.  Am.  Chem.  Soc.  1894, 
16.  483.) 

Fe2P.  Slowly  but  completely  sol.  in  HC1, 
or  dil.  H2SO4+Aq.  Sol.  in  hot  cone.  H2SO4, 
in  HNO3,  and  in  aqua  regia.  (Freese,  Pogg. 
132.  225.) 

Insol.  in  all  acids  except  in  a  mixture  of 
HNO3  and  HF.  (Maronneau,  C.  R.  1900, 
130.  657.) 

Fe3P4.  Very  slowly  sol.  in  hot  cone.  HC1  + 
Aq.  0.1  g.  dissolves  by  4  days'  heating  with 
HCl+Aq;  0.3  g.  dissolves  in  hot  cone.  H2SO4 
inll/2  hours;  0.4  g.  in  2  hours  in  HNO3+Aq. 
Quite  easily  sol.  in  aqua  regia  on  warming. 
(Freese.) 

Fe2P3.  Insol.  in  HC1,  HNO3  and  aqua 
regia.  Sol.  in  potassium  hypobromite  solu- 


IRON  SULPHIDE 


437 


tion.  (Granger,  Bull.  Soc.  1896,  (3)  15. 
1086.) 

Fe4P3.  Very  slowly  sol.  in  boiling  HCl-f- 
Aq.  Easily  sol.  in  HNO3  or  aqua  regia. 
(Struve,  J.  B.  1860.  77.) 

Mixture.    (Freese,  Pogg.  132.  225.) 

Almost  insol.  in  aqua  regia.  Sol.  in  fused 
alkali.  (Granger.) 

Fe3P.  Nearly  insol.  in  dil.  acids;  rapidly 
sol.  in  HNO3  or  aqua  regia;  decomp.  by  cone. 
HC1,  or  KOH+Aq.  (Schneider,  J.  B.  1886. 
2026.) 

Of  the  nine  iron  phosphides  described  the 
constitution  has  been  established  for  only 
two,  Fe3P  and  Fe2P. 

Fe3P.    Sol.  in  cone.  HC1. 

Fe2P.  Sol.  in  hot  aqua  regia.  Insol.  in 
other  acids.  (Le  Chatelier,  C.  R.  1909,  149. 
709.) 

Iron  selenide,  Fe2Se. 

Not  attacked  by  HNO3  or  acetic  acid.  SI. 
attacked  by  cone.  HC1.  Readily  attacked 
by  aqua  regia.  Sol.  in  HF.  (Vigouroux, 
C,  R.  1905,  141.  829.) 

FeSe+zH2O.  Sol.  in  HC1,  HNO3,  or 
HC2H3O2+Aq.  Insol.  in  alkalies,  or  (NH4)2S 
+Aq.  (Reeb,  J.  Pharm.  (4)  9.  173.) 

Fe2Se3.  Sol.  in  dil.  HC1,  or  HNO8+Aq  with 
evolution  of  H2Se.  Sol.  in  cone.  HNO3+Aq. 
(Little,  A.  112.  211.) 

Fe3Se4.  Decomp.  by  fuming  HNO3. 
(Fonzes-Diacon,  C.  R.  1900,  130.  1711). 

FerSeg.  Decomp.  by  fuming  HNO3. 
(Fonzes-Diacon,  C.  R.  1900,  130.  1711.) 

FeSe2.  Insol.  in  cone.  HC1;  decomp.  by 
fuming  HNO3.  (Fonzes-Diacon,  C.  R.  1900, 
130.  1711.) 

Iron  silicide,  Fe4Si. 

Difficultly  sol.  in  HCl+Aq;  easily  sol.  even 
in  dil.  HF+Aq.  (Hahn,  A.  129.  57.) 

Fe2Si.  Not  easily  sol.  in  cone.  HC1  and 
HNO3  but  readily  sol.  in  HF.  (Moissan, 
C.  R.  1895,  121.  623.) 

FeioSi9.  Sol.  in  hot  HCl+Aq  only  when 
most  finely  powdered.  (Hahn.) 

FeSi2.  Not  attacked  by  cone.  HF  or  H2SO4. 
(Hahn.) 

Sol.  in  cold  HF.  (de  Chalmot,  Am.  Ch.  J. 
1897,  19.  123.) 

Existence  questioned  by  Jouve,  (Bull.  Soc. 
1901,  25.  290-293). 

Fe3Si2.  Sol.  in  HF  and  in  fused  KNO3  and 
KNaCO3.  (de  Chalmot,  J.  Am.  Chem.  Soc. 
1895,  17.  924.) 

Iron  seraisulphide,  Fe2S. 

Sol.  in  dil.  acids  with  decomposition.  (Arf- 
vedson,  Pogg.  1.  72.) 

Ferrous  sulphide,  FeS. 

Decomp.  by  dil.  acids,  with  evolution  of 
H2S  and  without  separation  of  S,  except  with 
HNO3+Aq. 


+zH2O.  SI.  sol.  in  H2O,  especially  if  hot. 
(Berzelius.) 

1  1.  H2O  dissolves  70.1  x  1Q-6  moles  FeS  at 
18°.  (Weigel,  Z.  phys.  Ch.  1907,  58.  294.) 

Very  violently  decomp.,  even  by  dil.  acids. 
Sol.  in  H2S03+Aq.  Insol.  in  H9S,  or  (NH4)2S 
+Aq.  SI.  sol.  in  Na2S,  or  K2S+Aq.  Sol.  in 
Na2S  or  K2S  +Aq.  (de  Koninck,  Z.  angew. 
Ch.  1891.  204.) 

Insol.  in  NH4NO3,  or  NH4Cl+Aq.    (Brett.) 

Not  completely  pptd.  in  presence  of  Na  cit- 
rate. (Spiller.) 

Contrary  to  assertion  of  Persoz,  it  can  be 
nearly  completely  pptd.  in  presence  of 
Na4P2O7  by  (NH4)2S+Aq.  (Rose,  Pogg.  76. 
18.) 

Sol.  in  alkali  sulpho-molybdates,  -tung- 
states,  -vanadates,  -arsenates,  -antimonates, 
and  -stannates.  (Storch,  B.  16.  2015.) 

Sol.  in  KCN+Aq. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Solubility  of  FeS  in  sugar  solutions.     1  1. 
sugar  of  given  strength  dissolves  mg.  FeS. 


mg.  FeS 

°7  Sugar 

at  17.5° 

at  45° 

at  75° 

10 

3.8 

3.8 

5.3 

30 

7.1 

9.1 

7.2 

50 

9.9 

19.8 

9.1 

(Stolle,  Z.  Ver.  Zuckerind.  1900,  50.  300.) 

Colloidal. — A  very  dilute  solution  has  been 
obtained  which  coagulated  very  readily. 
(Winssinger,  Bull.  Soc.  (2)  49.  452.) 

Ferric  sulphide,  Fe2S3. 

Decomp.  by  dil.  HC1,  or  H2SO4+Aq  with 
evolution  of  H2S,  leaving  a  residue  of  FeS2. 

+  13/£H2O.  89!.  in  NH4OH+Aq,  also  in 
alcoholic  ammonia.  SI.  sol.  in  (NH4)2S+very 
dil.  Na2S2O3+Aq.  (Phipson,  C.  N.  30.  139.) 

Iron  bisulphide,  FeS2. 

Insol.  in  dil.  HC1,  or  H2SO3 + Aq.  Decomp. 
by  HNO3  or  aqua  regia  with  separation  of  S. 
Insol.  in  a  10%  solution  of  alkali  sulphide. 

Min.  Pyrite,  Marcasile.  Sol.  in  a  mixture 
of  Na2S  and  NaOH+Aq,  Na2S+Aq,  or  mix- 
ture of  Na2S  and  NaSH+Aq;  insol.  in  cold 
NaSH+Aq.  Marcasite  is  more  easily  sol.  in 
above  than  pyrite.  (Becker,  Sill.  Am.  J.  (3) 
33.  199.) 

Ferroferric  sulphide,  Fe8S9  or  Fe7S8. 

Min.  Pyrrhotile.  Sol.  in  dil.  acids  with  a 
residue  of  S.  Extremely  slowly  sol.  in  a  10% 
solution  of  alkali  sulphides.  (Terreil,  C.  R. 
69.  1360). 


438 


IRON  NICKEL  SULPHIDE 


lion  (ferrous)  nickel  sulphide,  2FeS,  NiS. 
Min.  Pentlandite. 

Ferrous  phosphorus  sulphide,  FeS,  P2S. 

(Berzelius.) 

2FeS,  P2S3.  Slowly  decomp.  by  H2O.  In- 
sol.  in  boiling  HCl+Aq;  decomp.  by  aqua 
regia.  (Berzelius,  A.  46.  256.) 

Iron  potassium  sulphide  (potassium  sulpho- 


ferrite),  K2Fe2 


mae  (po 

4  =  K2S,  ] 


Fe2S3. 


Insol.  in  cold  or  hot  H2O.  Violently  at- 
tacked by  dil.  acids.  Not  decomp.  by  boiling 
with  alkalies,  alkali  carbonates,  or  sulphides + 
Aq.  Decomp.  by  KCN,  or  Na2S2O3+Aq. 
(Preis,  J.  pr.  107.  16.) 

K2S,  2FeS.    (Schneider,  Pogg.  136.  460.) 

Iron   silver   sulphide    (silver   sulphoferrite), 

Ag2S,  Fe2S3. 

Not  attacked  by  dil.  HCl+Aq;  decomp.  by 
cone.  HCl+Aq.  (Schneider.) 

2Ag2S,  FeS,.    (Schneider,  Pogg.  138.  305.) 
Ag2S,  3FeS,  FeS2.    Min.  Sternbergite.    De- 
comp. by  aqua  regia. 

Iron  sodium  sulphide  (sodium  sulphoferrite), 

Na2Fe2S4+4H2O. 

Insol.  in  H->O.  Decomp.  by  very  dil.  acids. 
(Schneider,  Pogg.  138.  302.) 

Iron  sulphophosphide,  Fe2PS3. 

Attacked  by  acids  at  100°.  Decomp.  by 
boiling  NaOH+Aq.  (Ferrand,  A.  ch.  1899, 
(7)  17.  410.) 

Ferrous  telluride,  FeTe. 

Insol.  in  H2O;  sol.  in  acids.  (Fabre,  C.  R.' 
105.  277.) 

Kermes. 

See  Antimony  Znsulphide. 

"  Knallplatin  "  compounds. 
See  Fulminoplatinum  compounds. 

Krypton,  Kr. 

Absorption  by  H2O  at  t°. 


t 

Coefficient  of  absorption  det.  by  two 
series  of  experiments 

0 
10 
20 
30 
40 
50 

0.1249 
0.0965 
0.0788 
0.0762 
0.0740 
0.0823 

0.1166 
0.0877 
0.0670 
0.0597 
0.0561 
0.0610 

(Antropoff,  Roy.  Soc.  Proc.  1910,  83.  A.  480.) 


Lanthanic  acid. 

Barium  wetolanthanate,  Ba(H9La5Oi5)2. 
(Baskerville,  J.  Am.  Chem.  Soc.  1904,  26. 

79.) 

Lithium  metalanthanate,  LiH9La5Oi5+2H2O. 
(Baskerville.) 

Potassium      wetalanthanate,     KH9La5O15+ 

15H2O. 
Decomp.  by  H2O.    (Baskerville.) 

Sodium  metalanthanate,  NaH9La5Oi5+ 

4H2O. 

Almost  insol.  in  H2O,  but  decomp.  by  it. 
(Baskerville.) 

Dtsodium  te^ralanthanate*,  Na2La4O7. 
Insol.  in  H2O.    (Baskerville.) 

Lanthanicotungstic  acid. 

Ammonium  lanthanicotungstate,  2(NH4)2O, 

La2O3,  16WO3  +  16H2O. 
Ppt.    Insol.  in  H2O.    (E.  F.  Smith,  J.  Am. 
Chem.  Soc.  1904,  26.  1481.) 

Barium  lanthanicotungstate,  5BaO,  La2O3, 

16WO3+16H2O. 
Ppt.    (E.  F.  Smith.) 

Silver  lanthanicotungstate,  5Ag2O,  La2O3) 

16WO3+4H2O. 
Very  insol.  in  H2O.    (E.  F.  Smith.) 

Lanthanum,  La. 

Slowly  dtecomp.  cold,  rapidly  hot  H2O.  Not 
attacked  by  cold  cone.  H2SO4,  but  energet- 
ically by  cold  cone.  HNO3+Aq.  Sol.  in  dil. 
acids.  (Hillebrand  and  Nortdn,  Pogg.  166. 
633.) 

Lanthanum  bromide,  LaBr3+7H2O. 

Easily  sol.  in  H2O.  Not  very  sol.  in  ab- 
solute alcohol.  Insol.  in  ether.  (Cleve.  Sv. 
V.  A.  H.  Bih.  2.  No.  7.) 

Lanthanum  nickel  bromide,  2LaBr3,  3NiBr2+ 
18H20. 

Deliquescent.      (Frerichs   and   Smith,    A. 


191 


Jeliqu 
.355. 


Lanthanum  zinc  bromide,  2LaBr3,  3ZnBr2+ 
36H20. 

Very  deliquescent.    (F.  and  S.) 

Lanthanum  carbide,  LaC2.  I 

Decomp.  by  H2O  and  dil.  acids.  (Petters- 
son,  B.  1895,  28.  2422.) 

Sol.  in  cone.  H2SO4  and  dil.  acids;  insol.  in 
cone.  HNO3. 


LEAD 


439 


Sol.  in  fused  oxidizing  agents;  decomp.  , 
H2O  at  ordinary  temps.  (Moissan,  C.  R 
1896,  123.  149.) 

Lanthanum  chloride,  LaCl3. 

Anhydrous.     Deliquescent.    (Hermann.) 
Insol.  in  acetone.    (Naumann,  B.  1904,  37 

329.) 

+73^H2O.  Not  deliquescent.  (Zschiesche.^ 
Easily  sol.  in  alcohol.    (Hermann.) 

Lanthanum  mercuric  chloride,  2LaCl3,  HgCl 

+8/3H2O. 

Not  deliquescent.  Very  sol.  in  H2O 
(Marignac,  Ann.  Min.  (5)  15.  272.) 

Lanthanum  stannic  chloride. 
See  Chlorostannate,  lanthanum. 

Lanthanum  fluoride,  LaFH — H2O. 

Precipitate.    SI.  sol.  in  HCl+Aq.    (Cleve.) 

Lanthanum  hydrogen  fluoride,  2LaF3,  3HF. 

Precipitate.  (Frerichs  and  Smith,  A.  191 
355.) 

Does  not  exist.    (Cleve,  B.  11.  910.) 

Lanthanum  hydride,  La2H3. 

Decomp.  by  dil.  acids.  (Dinkier,  B.  24. 
1966.) 

LaH3.  Decomp.  by  H2O.  Sol.  in  acids 
with  evolution  of  H2.  Decomp.  by  alkalis. 
(Muthmann,  A.  1902,  325.  266.) 

Lanthanum  hydroxide,  La2O6H6. 

Insol.  in  H2O;  easily  sol.  in  acids;  insol.  in 
KOH,  or  NaOH+Aq. 

Sol.  in  citric  acid.  (Baskerville,  J.  Am. 
Chem.  Soc:  1904,  26.  49.) 

Lanthanum  zinc  iodide,  2LaI3,  3ZnI2+27H2O. 
Very  sol.  in  H2O.    (Frerichs  and  Smith,  A. 
191.  358.) 

Lanthanum  nitride,  LaN. 

Decomp.  by  H2O  with  evolution  of  NH3. 
Sol.  in  mineral  acids.  Decomp.  by  alkali. 
(Muthmann,  A.  1902,  325.  275.) 

Lanthanum  oxide,  La2O3. 

Easily  sol.,  even  when  ignited,  in  mineral, 
and  acetic  acids.  (Hermann.) 

Sol.  in  boiling  cone.  NH4Cl+Aq.  (Mos- 
ander.) 

Sol.  in  cold  cone.  NH4NO3+Aq.  (Damour 
and  Deville.) 

Insol.  in  (NH4)2CO3+Aq.     (Mosander.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Lanthanum  peroxide,  La4O0. 

Sol.  in  HC1,  H2SO4,  HNO3,  and  HC2H8O2  + 
Aq  with  decomp.  (Cleve,  Bull.  Soc.  (2)  43. 
359.) 

La2O5+zH2O.  Unstable.  Sol.  in  dil. 
H2SO4+Aq  with  decomp.  (Melikoff,  Z. 
anorg.  1899,  21.  71.) 


Lanthanum  oxybromide,  LaOBr. 
Ppt.    (Frerichs  and  Smith.) 

Lanthanum  oxychloride,  3La2O3,  2LaCl3. 

Insol.  in  H2O.  Difficultly  and  slowly  sol. 
in  HC1,  or  HNO3+Aq.  (Hermann.) 

LaOCl.  Boiling  H2O  dissolves  only  traces. 
(Frerichs  and  Smith.) 

Lanthanum  sulphide,  La2S3. 

Decomp.  by  H2O  and  acids.    (Didier.) 

Lanthanum  ^sulphide,  LaS2. 

Decomp. 'by  heat.  (Biltz,  Z.  anorg.  1911. 
71.  435.) 

Lead,  Pb. 

Lead,  in  contact  with  fhO  and  air  free  from  CCh, 
gives  a  solution  of  PbO  which  turns  litmus  blue  and 
turmeric  red,  and  is  turned  brown  with  EhS. 

H2p  which  has  been  boiled  does  not  dissolve  Pb  if 
there  is  no  access  of  air.  When  shaken  up  with  air  it 
dissolves  0.01  to  0.008%  PbO  in  2  hours.  Pure  spring 
water,  containing  1%  grains  salts  in  2  pounds  II2O  and 
no  CO2,  when  conducted  though  a  lead  pipe  150  feet 
long,  dissolves  so  much  lead  that  it  turns  brown  with 
H2S.  (Yorke,  Phil.  Mag.  J.  5.  82.) 

CO2  or  small  amts.  of  salts  prevent  the  solution  of 
Pb.  1  vol.  HzO  with  %  vol.  CC>2  dissolves  only  a  trace 
of  Pb.  Spring  PhO,  containing  in  10  pounds  1.21 
grains  NaCl  and  CaCb,  and  6.4  grains  CaCOs  dissolved 
in  CO2,  does  not  dissolve  lead.  (Yorke.) 

If  the  amt.  of  salts  in  solution  equals  g^  the  amt.  of 
EhO,  and  especially  if  they  are  carbonates,  very  slight 
amts.  of  Pb  are  dissolved.  (Christison,  Phil.  Mag.  J. 
21.  158.) 

CaCOs  dissolved  in  CO2  water  decreases  the  solu- 
bility of  Pb  more  than  any  other  salt. 

Distilled  EbO,  quietly  standing  in  a  closed  flask  with 
lead  and  air  free  from  COz,  deposits  white  flocks  of 
PbO2H2,  and  dissolves  7j,Jjjff  pt.  PbO.  The  solution  has 
an  alkaline  reaction,  (v.  Bonsdorff ,  Pogg,  41.  305.) 

Water  of  3°  hardness  does  not  take  up  enough  Pb  to 
become  injurious.  (Clarke,  J.  B.  1856.  608.) 

Soluble  carbonates  increase  the  solubility  of  Pb  in 
H2O  (Nevins,  C.  C.  1851.  608);  especially  (NH^COs. 
(Bottger.) 

Presence  of  H2SO4  decreases  the  solubility  of  Pb. 
(Horsford,  Chem.  Gaz.  1849.  247.) 

H2O  containing  K2SOi  takes  up  only  a  trace  of  Pb. 
(Wetzlar,  Schw.  J.  54.  324.) 

Presence  of  sulphates  diminishes  (Christison),  does 
not  diminish  (Graham,  Miller,  and  Hoffmann),  the 
action  of  H2O  on  Pb. 

CaSO4  protects  Pb,  but  it  is  attacked  by  much 
MgSO4.  (Nevins.) 

NaCl  +Aq  dissolves  only  a  trace  of  Pb. 

aflW  pt-  of  a  chloride  in  H2O  is  not  sufficient  to  pre- 
vent the  solubility  9f  Pb  in  H2O.  (Christison.) 

Presence  of  chlorides  increases  the  solubility.  (Gra- 
ham, Miller,  and  Hoffmann;  Nevins.) 

H2O  containing  KNOs  does  not  corrode  Pb. 

Nitrates  hinder  the  action  of  H2O.  (v.  Bonsdorff.) 
Nitrates  increase  the  action  of  H2O.  (Graham,  Miller, 
and  Hoffman.)  Nitrates  have  no  influence.  (Kersting.) 

10  Ibs.  of  H2O  dissolved  the  following  amts. 

'rom  Pb  pipes  in  24  hours:  if  distilled  H2O-f- 
1%  Na2C03,  0.38  grain  Pb;  if  Duna  water, 
0.19  grain  Pb;  if  canal  water,  0.15  grain  Pb;  if 
distilled  H2O  +  1%  NH4NO3,  0.15  grain  Pb: 
if  hard  well  water,  0.04  grain  Pb;  if  distilled 
H2O+1%  KNO3,  0.01  grain  Pb.  (Kersting, 
Dingl.  169.  183.) 

200  1.  Manchester  drinking  water  dissolved 
2.094  g.  from  1  sq.  metre  Pb  in  8  weeks;  9  1. 
well  water  dissolved  1.477  g.  from  1  sq.  metre 

Db  in  8  weeks;  11  1.  distilled  H2O  containing 


440 


LEAD 


are  dissolved  110.003  g.  from  1  sq.  metre  Pb 
in  8  weeks;  distilled  H2O  free  from  air  dis- 
solved 1.829  g.  from  1  sq.  metre  Pb  in  8 
weeks;  sea  water  dissolved  0.038  g.  from  1  sq. 
metre  Pb  in  8  weeks.  (Calvert  and  Johnson, 
C.  N.  16.  171.) 

A  lead  pipe  taken  up  in  Paris,  which  had 
been  exposed  to  action  of  ordinary  H2O  for 
200  years,  was  found  perfectly  smooth  and 
uncorroded.  (Belgrand,  C.  R.  77.  1055.) 

Pb  is  attacked  by  all  waters,  hard  or  soft; 
even  highly  calcareous  water  dissolves  some 
lead.  (Mayengon  and  Bergeret,  C.  R.  78. 484.) 

Pure  distilled  H2O  does  not  act  T>n  Pb,  but 
extremely  small  quantities  of  NH3,  HNO3, 
etc.  cause  an  action;  but  for  this  action  on  Pb 
the  presence  of  air  and  CO2  is  also  required. 
(Stallman,  Dingl.  180.  366.) 

100  ccm.  distilled  H2O  dissolved  3  mg.  from 
11.8  sq.  cm.  lead  in  one  week  when  air  with- 
out CO2  was  passed  through  the  solution.  8 
mg.  were  dissolved  when  the  air  contained 
CO2.  (Wagner,  Dingl.  221.  260.) 

Action  of  dil.  salt  solutions  on  lead.  In  500 
ccm.  of  the  solutions  containing  salt,  bright 
sheets  of  lead  of  5600  sq.  metres'  surface  were 
so  suspended  that  the  liquid  reached  all  parts 
of  the  metal  without  hindrance,  and  the  amts. 
dissolved  determined  after  24,  48,  and  72 
hours  of  action. 


Salt 

g.  salt  in 
100  ccm. 

mg.  Pb  dissolved 

without  CCh 

with  CO2 

KC1 

0.5 

21 

12 

NaCl 

0.5       • 

21 

12 

NH4C1 

1.0 

12 

5 

MgCl2 

0.83 

20 

35 

K2S04 

1.0 

0 

0 

KNO3 

1.0 

14 

20 

Na2CO3 

1.0 

0 

NaOH 

0.923 

430 

CaO2H2 

Saturated 

137 

Salt 

Grammes 
salt  per 
litre 

Dissolved  Pb  in  mg. 
per  litre 

after  24      48      72  hrs. 

NH4NO3 

0.020 

13.0 

25 

a       • 

0.040 

15.0 

32 

u 

0.080 

15.0 

KN03  + 

0.020 

NaN03 

0.050 

2.0 

2.0 

KN03+ 

0.040 

Na2S04 

0.212 

0.8 

1.0 

KNO3  + 

0.045 

K2CO3 

0.308 

0.3 

>KNO3+ 

0.070 

K2S04 

0.504 

0.5 

CaSO4 

0.252 

'6'.4 

0.8 

0.408 

0.4 

i!6 

K2C03 

0.310 

.... 

. 

6'.2 

« 

0.516 

.... 

_ 

0.2 

CaCl2 

0.250 

'6'.5 

6!s 

0.5 

« 

0.510 

0.3 

0.4 

Na2SO4 

0.200 

0.8 

it 

0.400 

0.5 

f  NH4N03+ 

0.020 

CaCl2 

0  060 

1.8 

NH4NO3+ 

0.020 

K2C08  + 

0.100 

0.4 

Na2SO4 

0.200 

'Na2S04+ 

0.200 

K2CO3+ 

0  040 

0.1 

CaCl2 

0.100 

Vater  from  L.  Katrine 

1.0 

1.0 

1.5 

distilled  water     . 

2.0" 

2.0 

3.0 

(Muir,  C.  N.  26.  294.) 

Action  of  salt  solutions  on  11.8  sq.  cm.  Pb 
in  one  week  while  air  either  with  or  without 
O2  was  passed  through  the  solution. 
Solubility  of  Pb  in  salt  solutions. 

100  ccm.  solutions  containing  the  given  amts. 
salts  dissolve  Pb  in  mg. : — 


(Wagner,  Dingl.  221.  260.) 

Solubility  of  Pb  in  salt  solutions. 

25  sq.  cm.  were  acted  upon  by  a  solution 
containing  0.2  g.  salt  in  a  litre  for  21  days. 

Three  series  of  experiments  were  carried  on. 
I.  In  corked  flasks.  II.  In  beakers  covered 
with  porous  paper;  diameter  of  mouth  of 
beaker  =  11.5  cm.  III.  In  basins  covered  with 
porous  paper;  diameter  of  mouth  of  basin  = 
14.5  cm.  IV.  In  corked  flasks  with  constant 
current  of  air.  V.  In  beakers  half  filled  and 
covered  with  porous  paper,  the  lead  being 
suspended  so  that  equal  amts.  of  surface  were 
above  and  beneath  the  liquid. 

The  amts.  in  mgs.  of  Pb  dissolved  were  as 
follows : — 


Salt  used 

I- 

n. 

ill. 

IV. 

1.5 
3.5 
5.0 
0.6 
2.0 

v. 

3^5 
2.5 
0.3 

NH4NO3 
KN03     . 

CaCl2      . 
(NH4)2S04       . 
K2CO3     . 
Dist.  H2O 

1.8 
1.6 
3.0 
0.7 
0.3 
1.5 

4.0 
0.5 
2.8 
1.3 
0.3 
0.8 

16.0 
6.0 
5.5 
16.0 
0.7 
4.2 

(Muir,  Chem.  Soc.  36.  660.) 

H2O  sat.  with  CO2  dissolves  0.012  g.  Pb  to 
a  litre  in  3  days.  (Marais,  C.  R.  77.  1529.) 

Action  of  H20  charged  with  CO2  under  760 
mm.  pressure  on  Pb.  3  mg.  of  Pb  were  dis- 
solved per  litre  in  24  hours,  and  the  amt.  was 
not  increased  by  further  action.  The  addition 
of  100  mg.  K2CO3+20  mg.  NH4NO3  to  a  litre 
prevented  all  action. 

Action  of  H2O  charged  with  CO2  under  6 
atmos.  pressure  on  Pb. 

14.8  mg.  were  dissolved  per  1.  in  24  hours, 
and  24  mg.  per  1.  in  48  hours. 

Action  of  various  salt  solutions  added  to 
above  solution  of  CO2  were  as  follows: — 


LEAD 


441 


mg.  salt 
per  1. 

mg.  Pb  dissolved 

niter 
24  hrs. 

after 

48  hrs. 

K2C03    .      .      . 
K2C03    .      .      . 
CaCl2     .      .      . 
NH4NO8      .      . 
NH4NO3      .      . 
Distilled  H20    . 

80 
160 

160 
16 
40 

13.2 

32^6 
5.0 
10.0 
14.8 

32.0 
6.0 
44.0 

35.Q 
24.0 

(Muir,  C.  N.  33.  125.) 

The  corrosion  of  Pb  by  ordinary  distilled 
H2O  depends  upon  the  presence  of  CO2  and  O. 
If  the  dissolved  CO  2  is  double  the  amt.  of  the 
dissolved  O,  the  action  is  most  energetic. 
When  CO2  is  wholly  absent  and  O  present, 
the  action  is  very  slight,  and  when  the  H2O 
contains  1%  or  more  vol.  %  CO2  with  normal 
amt.  of  oxygen,  there  is  no  visible  corrosion. 
Pure  distilled  H2O  containing  neither  O  nor 
CO2  has  no  action  on  Pb.  In  the  above  cases 
the  greater  part  of  the  Pb  remains  in  the 
form  of  a  white  ppt.  or  crust  on  the  Pb,  but 
in  the  case  where  O  and  C02  are  both  present 
in  the  ratio  of  1  : 2,  very  small  amts.  of  Pb 
go  into  solution  in  a  few  days;  the  amt.,  how- 
ever, diminishes  on  standing.  As  the  amt.  of 
CO2  increases,  the  amt.  of  Pb  dissolved  in  the 
H2O  also  increases. 

NH4OH  alone  does  not  protect  Pb  from 
corrosion,  but  when  in  combination  with  CO2 
the  action  is  much  diminished. 

CaO2H2,  and  NaOH+Aq  attack  Pb  much 
more  actively  in  absence  of  CO2  and  presence 
of  air.  In  absence  of  dissolved  O  neither 
CaO2H2  nor  NaOH  attacks  Pb. 

Na2CO3+Aq  in  absence  of  CO2  attacks  Pb 
slightly,  but  NaHCO3+Aq  has  not  the  slight- 
est action. 

CaH2(CO3)2+Aq  also  has  not  the  slightest 
action  on  Pb,  and  the  presence  of  CaCO3  and 
CO2  wholly  prevents  H2O  attacking  Pb. 

CaSO4+Aq  in  presence  of  air  forms  a  crust 
on  Pb,  but  no  Pb  is  found  in  solution,  but  if 
air  is  excluded  there  is  no  visible  action.  Pres- 
ence of  CO2  causes  a  strong  corrosive  action. 

H2O  containing  CaSO4  and  CaH2(CO3)2 
does  not  attack  Pb. 

The  above  reactions  are  not  in  the  least 
altered  by  the  presence  of  moderate  amts.  of 
nitrates,  chlorides,  or  ammonium,  or  organic 
compounds;  but  ammonium  salts  in  excess 
have  a  strong  solvent  action  on  Pb.  (Muller, 
J.  pr.  (2)  36.  317.) 

See  also  an  extended  report  of  the  action  of 
H2O  on  Pb  made  to  the  Water  Committee  of 
Huddersfield,  England,  in  1886,  by  Messrs. 
Crookes,  Odling,  and  Tidy. 

Very  extended  researches  are  published  by 
Cornelley  and  Frew  (Jour.  Soc.  Chem.  Ind.  7. 
15),  of  which  only  the  general  conclusions  can 
be  given  here. 


The  action  of  slaked  lime,  limestone,  sand 
calcium  silicate,  mortar,  etc.,  was  tested.  The 
results  were  as  follows: — 

1 .  In  nearly  all  cases  the  corrosion  is  greater 
with  free  exposure  to  the  air  than  when  air  is 
excluded.    The  difference  is  especially  great 
in  those  cases  where  the  greatest  action  on  the 
lead  takes  place.    Aluminum  hydroxide  and 
blue  clay  form  exceptions,  and  exert  a  greater 
corrosive  action  when  air  is  excluded.    In  the 
case  of  CaCO3,  old  mortar,  CaSiO3,  or  a  mix- 
ture of  CaCO3  and  CaO2H2,  the  exclusion  or 
presence  of  air  makes  no  appreciable  differ- 
ence. 

KNO3 + Aq  shows  a  peculiar  behaviour.  In 
the  presence  of  air  it  acts  nearly  as  much  on 
the  Pb  as  pure  H2O,  but  when  air  is  excluded 
it  exerts  nearly  as  much  retarding  action  as 
CaSi03. 

2.  In  the  presence  of  air  the  action  of  H2O 
on  Pb  is  considerably  increased  by  the  pres- 
ence of  NH4NO3  or  CaO2H4;  with  exclusion  of 
air,  by  CaSO4,  also  by  a  mixture  of  CaO2H2 
and  sand.     All  the  other  investigated  sub- 
stances, even  KNO3,  hinder  the  action  of  H2O 
on  Pb  either  with  or  without  exclusion  of  air. 

3.  CaO2H2-j-Aq  exerts  in  all  cases  a  much 
greater  corrosive  action  than  pure  H2O,  and 
although  this  action  is  diminished  by  sand 
yet  fresh  mortar  very  quickly  destroys  lead 
pipes  when  in  contact  therewith.    Old  mortar, 
on  the  other  hand,   and  also  CaSiO3   and 
CaCO3,  have  a  protective  action. 

4.  The  fact  is  very  important  that  sand, 
CaCO3,  old  mortar,  CaSiO3,  and  a  mixture  of 
sand  and  CaCO3  afford  considerable  protec- 
tion to  lead  against  H2O.    A  mixture  of  lime- 
stone and  sandstone  has  more  effect  than  the 
two  substances  separately. 

5.  CaSiO3  totally  prevents  the  corrosive 
action  of  KNO3  and  NH4NO3,  so  that  the 
lead  is  not  attacked  by  solutions  of  those  salts 
any  more  than  by  H2O  containing  CaSiO3 
alone.     Sand,  and  a  mixture  of  sand  and 
CaC03  have  a  similar  effect,  but  not  to  such 
a  degree. 

6.  The  protective  influence  of  CaCO3  does 
not  appear  to  depend  on  the  presence  of  CO2 
and  the  formation  of  CaH2(COs)2. 

7.  MgCO3  prevents  the  corrosion  of  Pb  as 
much  as  CaSiO3.    (Carnelley  and  Frew,  Jour. 
Soc.  Chem.  Ind.  7.  15.) 

Pb  in  contact  with  Zn  or  Fe  is  protected 
thereby  from  the  solvent  action  of  H2O,  and 
in  fact  the  action  is  nearly  null.  Sn,  on  the 
other  hand,  increases  the  action.  This  is  of 
importance  in  regard  to  the  use  of  tin-coated 
lead  pipes. 

The  presence  of  Ca  salts  does  not  influence 
the  action  of  the  H2O  on  Pb,  hard  or  soft  H2O 
provided  it  contains  CO2  having  a  strong 
corrosive  action.  Removal  of  air  from  H2O 
diminishes  the  solvent  action.  Simple  nitra- 
tion will  remove  all  Pb  from  H2O  if  suit- 
able filters  are  used.  (Flogel,  J.  B.  1888. 
2645.) 


442 


LEAD 


Pure  distilled  H2O  has  strong  corrosive 
action  on  Pb,  which  is  very  much  weakened 
by  addition  of  a  solution  of  CaCO3  in  carbonic 
acid  water,  but  the  presence  of  sulphates  in- 
crease the  action.  Pb  is  not  appreciably  at- 
tacked by  H2O  in  presence  of  chlorides  alone, 


but  very  strongly  when  CaSO4  is  also  present. 
H2O  containing  CO2  also  corrodes  Pb.  The 
conclusion  was  drawn  that  the  absence  of  ac- 
tion of  H2O  on  Pb  in  lead  pipes  is  due  to  the 
presence  of  traces  of  CaH2(CO3)2.  (Barbaglia 
and  Gucci,  C.  C.  1888.  934.) 


Solubility  in  H2O  containing  various  solids  in  solution. 


Water  used 


1 

2 

3 

4 

Water  alone,  unfiltered 

8.19 

12.98 

8.19 

4.09 

Water  alone,  filtered 

3.00 

4.09 

2.07 

2.32 

Water  containing  0  .  049  g.  NaCl  per  1.,  unfiltered 

1.36 

2.73 

0.68 

4.04 

"  "  filtered 

0.68 

1.50 

0.67 

1.36 

Water  containing  0.49  g.  Na2SO4  per  1.,  unfiltered 

3.41 

6.83 

2.05 

1.84 

"  "  filtered 

2.05 

3.41 

1.64 

1.77 

CaHCO3+Aq  containing  0.04  g.  CaO  as  carbonate  per  1. 
CaHCO3+Aq  with  NaCl 

2.45 
2.05 

3.14 
3.41 

2.63 
2.35 

5.70 
3.40 

CaHCO3+Aq  with  Na2SO4 

2.18 

3.32 

2.05 

3.16 

CaSO4+Aq  containing  0.095  g.  CaO  as  sulphate  per  1. 
CaS04+Aq  with  NaCl 

6.83 
5.46 

6.83 
6.57 

3.41 
3.51 

1.35 
1.50 

CaSO4+Aq  with  Na2S04 

4.78 

5.87 

3.69 

1.77 

Pts.  of  lead  per  100,000 


Column  1  gives  the  numbers  for  distilled  water  free  from  air;  column  2  for  distilled  water 
aerated  by  agitation  with  air;  column  3  for  water  continuously  aerated  by  passing  1  litre 
of  air  through  it  per  hour;  column  4  for  distilled  water  through  which  1  litre  of  air  and  400 
cc.  of  CO2  were  passed  per  hour  throughout  the  experiment.  (Antony  and  Benelli,  Gazz. 
ch.  it.  1896,  26,  (2)  97  and  352.) 


Almost  insol.  in  cold  HCl+Aq,  and  only  si. 
attacked  when  boiling.  Completely  sol.  in 
HNO3+Aq  if  not  too  cone.,  but  presence  of 
H2SO4  or  HC1  diminishes  the  solvent  power 
to  a  great  extent.  (Rose.) 

Granulated  Pb  is  si.  sol.  in  cone.  HCl+Aq; 
addition  of  PtCl4  makes  the  action  very  ener- 
getic. Dil.  HCl+Aq  may  also  be  used  with 
PtCl4.  •  (Millon,  C.  R.  21.  49.) 

HCl+Aq  of  1.2  sp.  gr.,  with  Pb,  gives  off 
H  at  ord.  temp.,  more  abundantly  when 
Jieated.  Evolution  of  H  is  hastened  by  plac- 
ing Cu  in  contact  with  the  Pb.  (Stolba,  J. 
pr.  94.  113.) 

Quickly  decomp.  by  hot  HCl+Aq,  slowly 
by  cold.  (Sharpies,  C.  N.  60.  126.) 

Scarcely  acted  upon  by  boiling  cone.  HC1+ 
Aq. 

Sol.  in  aqua  regia. 

HNO3+Aq  is  the  best  solvent,  but  Pb  is 
as  good  as  insol.  in  a  mixture  of  HNO3  and 
H2SO4.  (Berzelius.) 

Not  acted  upon  by  very  cone.  HNO3+Aq. 

Pb  is  only  si.  attacked  by  HNO3+Aq  of  any 
strength  below  15°.  Above  15°  it  is  most 
rapidly  attacked  by  a  rather  weak  acid. 
(Montemartini,  Gazz.  ch.  it.  22.  397.) 

Action  of  H2SO4  on  Pb. 

H2SO4  of  1.842  sp.  gr.  dissolves  201  g.  from 
1  sq.  metre  pure  lead  at  ordinary  temp, 
(time?),'  and  H2SO4  of  1.705  sp.  gr.  dissolves 
only  59  g. 

Slight  impurities  in  the  lead  lessen  this 


solubility.  (Calvert  and  Johnson,  Chem.  Soc. 
(2)  1.  66.) 

Strongly  attacked  by  99.8%  H2SO4  at  ord. 
temp,  with  exclusion  of  air.  (Lunge,  Dingl. 
261.  131.) 

When  0.2  g.  pure  Pb  was  heated  with  50 
ccm.  H2SO4  of  66°  B.  there  was  no  appreciable 
action  below  175°.  At  230-250°  all  the  Pb 
was  suddenly  converted  into  PbSO4,  which 
dissolved.  (Bauer,  B.  8.  210.) 

Lead  is  slowly  attacked  by  pure  cold  cone. 
H2SO4+Aq  (99.78%  H2SO4).  Lead  vessels 
which  held  the  H2SO4  were  gradually  de- 
stroyed by  long  standing.  (Napier  and  Tat- 
lock,  C.  N.  42.  314.) 

H2SO4+Aq  (20%)  does  not  evolve  H  under 
the  same  circumstances.  (Stolba.) 

Sol.  in  HC2H3O2+Aq  when  in  contact  with 
the  air. 

Strong  NH4OH+Aq  does  not  dissolve 
litharge;  but  lead  immersed  in  NH4OH+Aq 
3  days  gives  an  ammonia  solution  containing 
0.0139%  lead.  (Endemann,  Am.  Ch.  J. 
1897,  19.  892.) 

Somewhat  sol.  in  NaCl+Aq.  (Reichelt, 
Dingl.  172.  155.) 

NaCl+Aq  attacks  Pb  at  high  temp. 
(Lunge,  I  c.) 

Action  of  KC1O3.  KClO3+Aq  (6.3% 
KC1O3)  oxidised  64.31  g.  Pb  from  1  sq.  metre 
surface  by  boiling  7  hours;  KClO3+Aq  (25% 
KC1O3)  oxidised  151.12  g.  under  same  condi- 
tions; and  Ca(ClO3)2,  CaCl2+Aq  (20°  Baume) 


LEAD  BROMIDE 


443 


tions;  and  Ca(ClO3)2,  CaCl2+Aq  (20° 
Baume),  obtained  by  passing  C12  through 
CaO2H2-f-Aq,  oxidised  437.70  g.  (Lunge  and 
Deggeler,  Jour.  Soc.  Chem.  Ind.  4.  31.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 

Sol.  in  a  solution  of  K  in  liquid  NH3. 
(Kraus,  J.  Am.  Chem.  Soc.  1907,  29.  1562.) 

Y<L  ccm.  oleic  acid  dissolves  0.0592  g.  Pb  in 
6  days.  (Gates,  J.  phys.  Chem.  1911,  16. 
143.) 

Solubility  of  Pb  in  petroleum. 

If  b.-pt.  is  under  230°,  only  slightest  trace 
is  dissolved  in  4  months;  if  230-300°,  0.0026% 


Lead  bromide,  PbBr2. 

SI.  sol.  in  cold,  more  easily  in  hot  H2O, 
or  in  H2O  containing  HC1,  HNO3,  or  HC2H3O2 
(Lowig.) 

1  1.  H2O  dissolves  6  g.  PbBr2  at  10°;  addi- 
tion of  HBr  causes  a  ppt.  which  redissolves 
on  further  addition  of  HBr.  1000  pts.  of  a 
liquid  containing  720  pts.  HBr  dissolve  550  g. 
PbBr2.  This  solubility  increases  by  heating. 
(Ditte,  C.  R.  92.  718.) 

1  1.  H2O  dissolves  26.28  millimols.  PbBr2 
•at  25.2°.  (von  Ende,  Z.  anorg.  1901,  26.  159). 


in  4  months;  if  over  300°,  0.0244%  in  4  months 
in  4  months;  if  over  300°,   0.0244%  in  4 
months. 

Solubility  of  Pb  in  commercial  oil  of  turpen- 
tine and  resin  oil. 

t 

G.  PbBr2 

0 
15 
25 
35 
45 
55 
65 
80 
95 
MOO 

0.4554 
0.7305 
0.9744 
1.3220 
1.7457 
2.1376 
2.5736 
3.3430 
4.3613 
4.7510 

Temp. 

%  Pb  dissolved 

in  8  days 

in  14  days 

Fresh  oil  of 
turpentine    . 
Old  oil  of  tur- 
pentine   . 
Fresh  oil  of 
turpentine    . 
,Old  oil  of  tur- 
pentine   . 
Fresh  oil  of 
turpentine    . 
Old  oil  of  tur- 
pentine  . 
Fresh  resin  oil 
Old 
Fresh 
Old 
Fresh 
Old 

15-20° 
15-20 
100 
100 
130-150 

130-150 
15-20 
15-20 
100 
100 
130-150 
130-150 

sl.  trace 
0.0522 
0.265 
0.982 
0.938 

1.738 
trace 
0.073 
0.380 
1.190 
1.050 
2.208 

0.0722 
0.1435 
0.715 
1.851 
2.045 

4.083 
0.024 
0.185 
0.880 
2.711 
2.065 
4.740 

*  By  extrapolation. 
(Lichty,  J.  Am.  Chem.  Soc.  1903,  25.  474.) 

SI.  sol.  in  H2O. 
8.34  x  10.  1  gram,  are  dissolved  in  1  liter  of 
sat.  solution  at  20°.     (Bottger,  Z.  phys.  ch. 
1903,  46.  603.) 

Solubility  of  PbBr2  in  HNO3+Aq  at  25.2°. 
S  =  solubility  in  millimols  per  litre. 

HNO3  normal                                      S 

0.001                                  39.11 
0.01                                   39.87 
0.051                                 42.56 
0.04KNO3+ 
0.01HNO3                       42.77 

(Engler  and  Kneis,  Dingl.  263.  193.) 

Pb  is  strongly  attacked  by  oil  of  turpentine. 
(Am.  Chem.  4.  289.) 

The  fatty  oils  dissolve  Pb  in  considerable 
amt.  (Macadam,  J.  B.  1878.  1169.) 

Not  attacked  by  sugar +Aq.  (Klein  and 
Berg,  C.  R.  102.  1176.) 

Lead  potassium  amide. 
See  Potassium  ammonoplumbite. 

Lead  azoimide,  basic,  PbO,  PbN6. 

Insol.  in  H2O.    (Wohler,  B.  1913,  46.  2054.) 

Lead  azoimide,  PbN6. 

Insol.  in  cold  H2O;  much  less  sol.  in  boiling 
H2O  than  PbCl2.  1  1.  H2O  dissolves  about  1A 
g.  PbN6.  Easily  sol.  in  warm  HC2H3O2+Aq. 
Insol.  in  cone.  NH4OH+Aq.  (Curtius,  B.  24. 
3344.) 


(von  Ende,  Z.  anorg.  1901,  26.  162.) 

Slowly  sol.  in  cold,  easily  in  warm  NH4C1, 
or  NH4NO3+Aq.  (Wittstein.) 

Not  pptd.  in  presence  of  Na  citrate. 
(Spiller.) 

Insol.  in  H2O  containing  Pb(NO3)2.  (von 
Ende,  Z.  anorg.  1901,  26.  159.) 

Insol.  in  benzene.  (Franchimont,  B.  16. 
387.) 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  828.) 

Insol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1370.) 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate  (Naumann, 
B.  1910,  43.  314.) 

Difficultly  sol.  in  acetone.  (Naumann,  B. 
1904,  37.  4328.) 

+3H2O.    (Ditte,  I.  c.) 


444 


LEAD  HYDROGEN  BROMIDE 


Lead  hydrogen   bromide,    5PbBr2,    2HBr+ 

10H2O. 
Sol.  in  HBr+Aq.    (Ditte,  C.  R.  92.  718.) 

Lead  magnesium  bromide.  PbBr2,  2MgBr2  + 

16H2O. 

Very  deliquescent.  Decomp.  immediately 
by  H2O  or  alcohol.  (Otto  and  Drewes,  Arch. 
Pharm.  229.  585.) 

Lead  potassium  bromide  (potassium  bromo- 

plumbite,  PbBr2,  KBr+H2O. 
(Remsen  and  Herty,  Am.  Ch.  J.  14.  124.) 
+-H2O.     (Wells,  Sill.  Am.  J.  145.  129.) 
PbBr2,  2KBr.    Sol.  in  a  little  H20  without 

decomp.,   but   decomp.   by   an   excess   with 

separation  of  PbBr2.    (Lowig.) 

+H2O.    (Wells,  Sill.  Am.  J.  145.  129.) 
2PbBr2,  KBr.    (Wells.) 

Lead    potassium    perbromide,    K3Pb2Br8  + 

4H2O. 

Decomp.  by  H2O  and  alcohol.  (Wells,  Z. 
anorg.  4.  340.) 

Lead  rubidium   bromide,   PbBr2,   2RbBr+ 


(Wells,  Sill.  Am.  J.  146.  34.) 
2PbBr2,  RbBr.    (Wells.) 

Lead  sodium  bromide. 

Decomp.  by  H2O.    (Lowig.) 

Lead  bromochloride,  PbBrCl  =  PbBr2,  PbCl2. 

Can  be  recrystallised  from  H20  without 
decomp.  (lies,  C.  N.  43.  216.) 

3PbCl2,  PbBr2.  Sol.  in  H2O  with  decomp. 
Sol.  in  HC1  and  in  HBr.  Insol.  in  cold  al- 
cohol; si.  sol.  in  boiling  alcohol.  (Thomas, 
C.  R.  1899,  128.  1235.) 

Lead  bromoiodide,  PbBrI  =  PbBr2,  PbI2. 

Decomp.  by  H2O.  Cryst.  from  a  solution 
of  PbI2  in  HBr.  (Grissom  and  Thorp,  Am. 
Ch.  J.  10.  229.) 

3PbBr2,PbI2.  Decomp.  by  H2O.  (Thomas 
C.  R.  1899,  128.  1236.) 

6PbBr2,  PbI2.    (G.  and  T.) 

Lead  bromosulphide,  PbBr2,  PbS. 

Properties  as  chlorosulphide.  (Parmentier.) 

Lead  chloride,  PbCl2. 

Slowly  sol.  in  135  pts.  H2O  at  12.5°,  and  in  a  much 
smaller  quantity  of  hot  H2O.  (Bischof.) 

Sol.  in  30  pts.  cold,  and  22  pts.  hot  H2O.    (Wittstein.) 

Sol.  in  30  pts.  H2O  at  18.75°.     (Abl.) 

100  pts.  H2O  dissolve  4.59  pts.  PbCb  at  15.5°.  (Ure's 
Diet.) 

100  pts.  H2O  dissolve  0.9712  pt.  PbCl2  at 
20°.  (Formanek,  C.  C.  1887.  270.) 

100  pts.  H2O  dissolve  0.946  pt.  PbCl2  at 
17.7°.  (Bell,  Chem.  Soc.  (2)  6.  355.) 

Sol.  in  105.2  pts.  H2O  at  16.5°.  (Bell,  C.  N. 
16.  69.) 


t° 

G.  PbCl2 

0 

0.6728 

15 

0.9090 

25 

1.0842 

35 

1.3244 

45 

1.5673 

55 

1.8263 

65 

2.1265 

80 

2.6224 

95 

3.1654 

*100 

3.3420 

100  pts.  H2O  dissolve  0.8  pt.  PbCl2  at  0°; 
1.18  pts.  at  20°;  1.7  pts.  at  40°;  2.1  pts.  at 
55°;  3.1  pts.  at  80°.  (Ditte,  C.  R.  92.  718.) 

1  1.  H2O  dissolves  38.80  millimols.  PbCl2  at 
25.2°.  (von  Ende,  Z.  anorg.  1901,  26.  148.) 

9.61  x  10-1  gram  are  dissolved  in  1  liter  of 
sat.  solution  at  20°.  (Eottger,  Z.  phys.  ch. 
1903,  46.  603.) 

Solubility  in  H2O. 
100  g.  H2O  dissolve  g.  PbCl2  at  t°. 


*  By  extrapolation. 
(Lichty,  J.  Am.  Chem.  Soc.  1903,  25.  474.) 

33.6  millimols.  Pb  are  dissolved  in  1  liter 
H2O  at  18°.  (Pleissner,  C.  C.  1907,  II.  1056.) 

1  1.  H2O  dissolves  77.76  milliequivalents 
PbCl2  at  25°.  Sp.  gr.  of  the  solution  25°/4°  = 
1.0069.  (Harkins  and  Winninghoff,  J.  Am. 
Chem.  Soc.  1911,  33.  1816.) 

0.0388  mol.  mg.  PbCl2  are  sol.  in  1  1.  H2O. 
(Kernot  and  Pomilio,  Soc.  R.  Napoli,  1912, 
(3),  XVII,  353.) 

A  colloidal  modification  is  sol.  in  hot  water 
to  give  cryst.  modification.  (Van  de  Veide, 
Ch.  Z.  1893,  17.  1908.) 

Solubility  in  H2O  is  not  much  increased  by 
the  addition  of  acids.  (Fresenius.) 

Sol.  in  cone.  HCl+Aq,  from  which  it  is 
pptd.  by  H2O,  but  less  sol.  in  dil.  HCl+Aq 
than  in  H2O.  (Berzelius.) 

Sol.  in  1636  pts.  H2O  containing  HC1. 
(Bischof.) 

Sat.  solution  of  PbCl2  in  HCl+Aq  of  1.116 
sp.  gr.  contains  2.566%  PbCl2  at  16.5°. 

Solubility  in  HCl+Aq.  100  pts.  liquid  con- 
taining pts.  HC1  of  1.1162  sp.  gr.  in  100 
pts.  H2O  dissolve  pts.  PbCl2  at  17.7°. 


Pts. 

Pts. 

Pts. 

Pts. 

Pts. 

Pts. 

HCl 

PbCl2 

HCl 

PbCl2 

HCl 

PbCl2 

1 

0.347 

8 

0.099 

50 

0.356 

2 

0.201 

9 

0.096 

60 

0.559 

3 

0.165 

10 

0.093 

70 

0.933 

4 

0.145 

15 

0.090 

-80 

1.498 

5 

0.131 

20 

0.111 

90 

2.117 

6 

0.107 

30 

0.151 

100 

2.900 

7 

0.100 

40 

0.216 

•• 

... 

(Bell,  Chem.  Soc.  21.  350.) 

LEAD  CHLORIDE 


445 


Solubility  of  PbCl2  in 

HCl. 

Solubility  of  PbCl2  in  HCl  at  18°. 

Amt.  HCl 
in  100  pts. 
H20 

Amount  PbCh  dissolved  in  1000 
liquid 

pts.  of 

HCl  Normality 

G.  PbCh  per  1. 

At  0° 

At  20° 

At  40° 

At  55° 

At  80° 

0 

0.0001 
0.0002 
0.0005 
0.00102 
0.0102 

9.34 

9.305 
9.300 
9.243 
9.200 
8.504 

0.0 

5.6 
10.0 
18.0 
21.9 
31.5 
46.0 

8.0 
2.8 
1.2 
2.4 
4.7 
11.9 
29.8 

11.8 
3.0 
1.4 
4.8 
6.2 
14.1 
30.0 

17.0 
4.6 
3.2 
7.2 
10.4 
19.0 

21.0 
6.5 
5.5 
9.8 
12.9 
24.0 

31.0 
12.4 
12.0 
19.8 

23.8 
38.0 

(Pleissner,  Arb.  Kais.  Gesundamt.  1907,  26. 

384.) 

Sol.  in  hot,  insol.  in  cold  cone.  H2SO4. 
(Hayes.) 
"Sol.  in  dil.  HNO3+Aq,  from  which  it  is 
pptd.  by  HCl+Aq.    (Gladstone.) 
Easily   and    completely   decomp.    by   hot 
HNO3+Aq.    (Wurtz.) 

Solubility  of  PbCl2  in  HNO3+Aq  at  25.2°. 
S  =  solubility  in  millimols  per  litre. 

(Ditte,  C.  I 
Solubility  in  HCl+Aq  j 

PbCl2  in  mgs.  in  1( 
mols.  HCl  in  ditto 

I.  92.  718.) 
it  0°     PkCl2  _  i^mrie 

2 

)  ccm.  solution; 

HC1  = 

PbCl2 
2 

HCl 

PbCls 

HCl 

2 

0.42 
0.22 
0.135 
0.11 
0.105 
0.099 
0.090 
0.08 

0. 
0.35 
0.675 
1.125 
1.6 
2.3 
3.4 
4.5 

0.072 
0.088 
0.100 
0.209 
0.95 
1.5 
1.9 
3.01 

5.8 
11.7 
29.5 
46.7 
73.5 
89.0 
96.0 
111.5 

HNOs  formal 

S 

0.001 

0.01 
0.051 
0.04KNO3+ 
O.OlHNOs 

38.87 
39.71 
42.92 

43.36 

It  is  seen  that  very  little  HCl+Aq  is  suffi- 

cient  to  diminish  solubility  very  considerably, 
and,  that  on  further  addition  of  HCl+Aq,  the 
solubility  is  nearly  constant,  and  increases  fi- 
nally very  much  when  large  amts.  of  HCl+Aq 
are  present.  (Engel,  A.  ch.  (6)  17.  359.) 


(von  Ende,  Z.  anorg.  1901,  26.  162.) 

Solubility  of  PbCl2  in  NH4Cl+Aq  at  25.20°. 
S  =  solubility  in  millimols  per  litre. 


Solubility  of  PbCl2  in  HCl+Aq  at  25°. 

NH4C1  normal                                     S 

G.  HCl 

G.  PbCl2           G.  HCl 

G.  PbCh 

0  25                              9  47 

perl. 

per  1.                   per  1. 

perl. 

0  50                              7  11 

0 

10.79                  3 

5.0 

1.0                                4.35 

0.5 
1. 

9.0                   6 
7.6                 10 

3.1 

1.8 

(von  Ende,  Z.  anorg.  1901,  26.  152.) 

2. 

6.0 

Solubility  of  PbCl2+NH4Cl  at  22°. 

(Noyes,  Z.  phys.  Ch.  1892,  9.  623.) 

Solubility  of  PbCl2  in  HCl+Aq  at  25.20°. 
S  =  solubility  in  millimols  per  litre. 

G.  equiv. 
per  1.  H2O 
NH<C1 

G.  equiv.  per 
100  cc.  H2O 
PbCl2 

G.  equiv. 
per   1.  H2O 
NH4C1 

G.  equiv.  per 
100  cc.  H2O 
PbCh 

HCl  normal 

S 

HCl  normal 

S 

0.0 

7.49xl03 

1.0 

0.758x10  3 

0.0000 
0.0009 
0.0022 
0.0030 
0.0045 
0.0091 
0.0114 
0.0151 
0.0226 
0.0302 

38.80 
38.66 
38.20 
37.94 
37.35 
35.80 
34.99 
33.75 
31.46 
29.32 

0.3714 
0.5142 
0.7386 
1.026 
1.538 
2.051 
2.564 
3.085 
3.718 
5.0 

6.35 
5.37 
4.73 
4.41 
4.61 
5.18 
6.25 
7.78 
8.16 
19.38 

0.1 

0.2 
0.3 
0.4 
0.5 
0.55 
0.6 
0.65 
0.7 
0.8 

On 

3.10 
.916 
.508 
.348 
.263 
.189 
.092 
1.012 
0.956 
0.837 

07QO 

1.2 
1.5 
2.0 
2.5 
3.0 
4.0 
5.0 
6.0 
7.0 
7.29* 

0.707 
0.671 
0.695 
0.812 
0.968 
1.502 
2.338 
3.580 
5.628 
6.46 

0.0452 

25.46 

7.5 

65.86 

0.0910 

17.12 

10.0 

141.35 

*  Saturated 

0.1850 

10.12 

12.05 

164.3 

(Bronsted,  Cong.  Appl.  Chem.  1909,  Sec.  X, 

(von  Ende,  Z.  anorg.  1901,  26.  148.) 

110.) 

446 


LEAD  CHLORIDE 


Solubility  in  NH4Cl+Aq  at  t°. 

Much  more  sol.  in  HgCl2+Aq  than  in  H2O. 

Grammes 
HgCh  in 
100  ccm. 

Grammes 
PbCl2 
dissolved 

After  sub- 
tracting amt. 
dissolved  by 
H2O  alone 

Calculated 
no.  of 
grammes  for 
100  g.HgCh 

t 

G.  PbCl2  in 
100  g.  of 
the  solution 

G.  NEUCl 

in  100  g.  of 
the  solution 

Solid  phase 

17° 

0.89 
0.21 
0.16 
0.14 
0.076 
0.078 
0.078 
0.098 
0.34 
0.64 
0.52 
0.33 
0.30 
0.0 

0.0 
0.96 
1.43 
2.40 
3.48 
4.23 
4.93 
12.36 
22.33 
26.49 
26.68 
26.91 
27.03 
27.14 

PbCl2 
eutectic-pt. 
[2PbCl2,  NH4C1 
eutectic-pt. 
NH4C1 

0 

4 
2 
1 
0.5 
0.25 
0.125 

0.9712 
1.8972 
1.4874 
1.2272 
1.0808 
1.0192 
0.9926 

0*9350 
0.5208. 
0.2600 
0.1134 
0.0500 
0.0226 

23^37 
26.04 
26.00 
22.68 
20.00 
18.08 

(Formanek,  C.  C.  1887.  270.) 
Solubility  of  PbCl2  in  Pb(NO3)2+Aq  at  20°. 

G.  equiv.  per  1. 

Pb(N03)2 

PbCh 

0.0 

0.2                  ';: 

0.0777 
0.0832 

50° 

1.69 
1.08 
0.67 
0.58 
0.48 
0.49 
0.71 
1.76 
3.31 
3.96 
2.65 
1.62 
0.32 
0.0 

0.0 
0.51 
1.45 
2.45 
4.86 
12.45 
19.42 
27.16 
31.90 
33.56 
33.62 
33.88 
34.14 
34.25 

PbCl2 
eutectic  pt. 
2PbCl2,  NH4C1 
eutectic  pt. 
NH4C1 

(Noyes,  Z.  phys.  Ch.  1892,  9.  623.) 

Solubility  in  Pb(NO3)2+Aq  at  25°. 
C  =  concentration  of  Pb(NO3)2  in  Pb(NO3)2 
+Aq  expressed  in  milliequivalents  per  1. 
di=Sp.  gr.  of  Pb(NO3)2+Aq  at  25°. 
S  =  Solubility  of  PbCl2  in  Pb(NO3)2+Aq 
expressed  in  milliequivalents  per  1. 
d2  =  Sp.  gr.  25°/4°  of  PbCl2+Pb(NO3)2  + 
Aq. 

C 

di 

s 

d2 

20.020 
50.063 
99.660 

1.0008 
1.0045 
1.0119 

76.75 
76.64 
77.98 

1.0095 
1.0139 
1.0210 

100° 

3.10 
2.02 
1.85 
1.80 
1.76 
1.98 
4.54 
8.32 
11.40 
12.67 
12.50 
11.60 
10.70 
9.88 
9.26 
4.21 
3.06 
1.61 
0.0 

0.0 
1.32 
5.33 
6.01 
8.59 
13.19 
26.08 
32.64 
36.29 
37.62 
38.14 
38.32 
38.66 
40.22 
41.90 
42.91 
43.20 
43.42 
43.51 

PbCl2 
eutectic  pt. 
l2PbCl2,  NH4C1 
eutectic  pt. 
1  PbCl2,  2NH4C1 
eutectic  pt. 
NH4C1 

(Harkins  and  Winninghof,  J.  Am.  Chem.  Soc. 
1911,  33.  1816.) 

Solubility  of  PbCl2  in  Pb(NO3)2-f  Aq  at  25°. 

G.  Pb(N03)2per  1. 

%  PbCl2 

0 
3.31 
6.62 
33.12 

82.80 

1.09 
1.10 
1.05 
1.11 
1.29 

(Armstrong  and  Eyre,  Proc.  Roy.  Soc.  1913, 
(A)  88.  234.) 

Solubility  of  PbCl2  in  KCl+Aq  at  25.20°. 
S  =  Solubility  in  millimols  per  litre. 

KCl  normal 

s 

KCl  normal 

s 

These  results  show  that  the  double  salt 
PbCl2,  2NH4C1  can  only  exist  in  aqueous 
solution  at  temperature  above  70°. 
(Demassieux,  C.  R.  1913,  166.  894.) 

0.0000 
0.001 
0.0025 
0.0049 
0.0049 
0.0099 
0.0200 
0.0599 

38.80 
38.32 
37.85 
37.02 
37.02 
35.28 
32.16 
22.62 

0.0999 

0.5006 
0.7018 
0.9991 
0.9991 
1.5018 
2.0024 
3.0036 

16.90 
7.40 
7.38 
4.90 
4.90 
4.83 
5.56 
9.74 

(von  Ende,  Z.  anorg.  1901,  26.  151.) 

LEAD  CHLORIDE 


447 


Solubility  of  PbCl2+KCl  in  H2O  at  20°. 

A  study  of  the  equilibrium  between  lead 

Values  =  g.  equivalents. 

chloride  and  sodium  chloride  in  aqueous  solu- 
tion at  13°,  50°  and  100°  shows  that  at  none 

In  1000 
g.  solution 

In  1000  g.  H20 

Solid  phas6 

of  these  temp,   do  these  chlorides  form  a 
double  salt.     (Demassieux,  C.  R.  1914,  158. 

PbCb 

KCl 

PbCh 

KCl 

702.) 

28.0 

4.57 

PbCl2,  KCl. 

Solubility  in  salts+Aq  at  25°. 

V3H2O+KC1 

Concentration  of 

the  salt. 

Solubility  of  PbCl2 

17.80 

3.18 

23.42 

4.18    } 

oalt  used 

Equivalents  per 

Equivalents  per  liter 

16.56 

3.05 

21.50 

3.96 

liter 

15.50 
14.76 
13.96 

2.91 

2.77 
2.66 

19.85 
18.66 

17.48 

3.73 
3.50 
3.33 

PbCl2,  KCl. 

V3H20 

None 

HC1 
tt 

0 

0.05 
01 

0.07770 
0.04786 
0  03243 

13.16 
13.08 
12.94 

2.47 
2.45 
2.40 

16.17 
16.06 
15.80 

3.03 
3.01 
2.93 

KCl 

(( 

.    1 

0.2 
0.05 
0.1 

\J  .  v/O^-r±O 

0.01927 
0.0482 
0.0341 

(( 

00 

0091Q 

12.96 
12.86 

2.36 
2.35 

14.92 
15.63 

2.87    ] 
2.86 

MgCl2 

.  £ 

0.05 
0  1 

.  i  '_  i  .' 
0.0503 

12.44 
11.84 

2.30 
2.29 

15.03 
14.30 

2.78 
2.77 

CaCl2 

\J  •  JL 

0.05 
0.  1 

0^0503 

11.38 

2.24 

13.70 

2.70 

ft 

02 

0.0219 

10.60 
11.98 

2.20 
2.29 

12.72 
14.35 

2.64 
2.62 

MnCl2 
a 

"  •  ^ 

0.05 
0.1 

0'0501 
0  0349 

10.46 

2.14 

12.47 

2.55 

(( 

00 

0  0917 

10.22 

9.82 
9.34 

2.10 
2.04 
.965 

12.13 
11.60 
10.96 

2.49 
2.41 
2.31 

ZnCl2 
CdCl2 

.  £i 

0.2 
0.05 
0.1 

\J  .  \J£  1  / 

0.0220 
0.0601 
0.0481 

8.94 

.884 

10.42 

2.20 

« 

0.2 

0.0355 

7.86 

.575 

8.92 

1.79 

7.72 

.526 

8.72 

.744 

(Noyes,  Z.  phys.  Ch.  1892,  9.  623.) 

7.66 

.404 

8.56 

.570 

7.46 

.324 

8.29 

.472 

2PbCl2,  KCl 

Sol.  in  KOH+Aq.    (Rose.) 

7.36 

.224 

8.11 

.348 

Less  sol.  in  dil.  salt  solutions  than  in  H2O, 

7.38 

.223 

8.13 

.347 

especially  CaCl2+Aq;  sol.  in  534  pts.  H2O 

7.30 

.127 

7.98 

.231 

containing  CaCl2.    (Bischof.) 

7.34 

.122 

8.01 

.225 

More  sol.  in  Na2S2O3+Aq  than  in  H2O,  but 

7.36 

.059 

8.00 

.152 

not  as  sol.  as  AgCl.    (Herschell,  1819.) 

7.48 

.022 

8.10 

.107 

More  sol.  in  NaC2H3O2+Aq  than  in  H2O. 

7.52 

0.988 

8.13 

.068 

(Anthon.) 

7.70 

0.930 

8.28 

.000 

Easily  sol.  in  NH4NO3+Aq. 

7.82 

0.880 

8.38 

0.943 

SI.  sol.  in  liquid  NH3.    (Franklin,  Am.  Ch. 

8.24 

0.821 

8.79 

0.875 

J.  1898,  20.  828.) 

8.42 

0.783 

8.96 

0.833 

Insol.  in  cone,  alcohol.     (Wittstein.)     In- 

8.84 

0.719 

9.36 

0.761 

sol.  in  94%  alcohol;  very  si.  sol.  in  cold  or  hot 

9.54 

0.639 

10.03 

0.672 

76%  alcohol. 

10.68 

0.575 

11.18 

0.602 

Solubility  in  alcohol  at  25°. 

12.32 

0.523 

12.85 

0.545. 

Alcohol  =  g.  mol.  alcohol  in  1  1.  of  solvent. 

PbCl2  =  g.  mol.  PbCl2  in  1  1.  of  solution. 

12.38 

0.503 

12.88 

0.523] 

Alcohol     -4           2            1          V2          V* 

12.36 

0.483 

12.85 

0.502 

PbCl2      0.0172  0.0257  0.0298  0.0330  0.0338 

12.56 

0.475 

13.04 

0.497 

12.48 

0.458 

12.95 

0.475 

PbCl2 

Alcohol      Vs           0 

12.24 

0.375 

13.65 

0.387 

PbCl2      0.0367  0.0388 

14.52 

0.299 

14.88 

0.306 

(Kernot  and  Pomilio.  Soc.  R.  Napoli,  (3)  17. 

19.00 

0.195 

19.33 

0.199 

353.) 

(Bronsted,  Z.  phys.  Ch.  1912,  80.  208.) 

PbCl2  is  sol.  in  120  pts.  pure  H2O,  but  on 
adding  5%  NaCl  437  pts.  are  required  to 
effect  solution.  When  PbCl2  is  digested  with 
cone.  NaCl+Aq,  1  pt.  dissolves  in  129  pts.  of 
the  liquid. 


Insol.  in  benzene.  (Franchimont,  B.  16. 
387.) 

Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.  257.) 

Insol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1370.) 

Insol.   in  methyl  acetate   (Naumann,    B. 


448 


LEAD  CHLORIDE 


1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

Insol.  in  methylal.  (Eidmann,  C.  C.  1899, 
II,  1014.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Glycerine  dissolves  1.995%  PbCl2. 

1  pt.  glycerine  +1  pt.  H2O  dissolves  1.32% 

1  pt.  glycerine+3  pts.  H2O  dissolves  1.0365 
%  PbCl,. 

Glycerine  containing  87.5%  H2O  dissolves 
0.91%  PbCl2.  (Piesse,  B.  7.  599.) 

Solubility  of  PbCl2  in  mannite  +Aq  at  25°. 

Mannite  =  g.  mol.  mannite  in  1  1.  of  solvent. 

PbCl2  =  g.  mol.  PbCl2  in  1  1.  of  solution. 
Mannite     l/2          */4  V8         Vie       Vs2 

PbCl2      0.0408  0.0403  0.0394  0.0384  0.0385 

Mannite     Ve4  0 

PbCl2      0.0377  0.0388 

(Kernot  and  Pomilio,  Soc.  R.  Napoli,  (3)  17. 

353.) 
Min.    Cotunnite. 

Lead  ^rachloride,  PbCl4. 
•     Sol.    in    H2O    with    subsequent    decomp. 
(Rivot,  Beudant,  and  Daguin,  Ann.  Min.  (5) 
4.  239.) 

Obtained  in  a  pure  state  by  Friedrich.  Sol. 
in  a  little  cold  H2O,  but  is  decomp.  by  warm- 
ing or  diluting.  Miscible  with  cone.  HC1+ 
Aq;  not  attacked  by  cone.  H2SO4  even  on 
warming.  (Friedrich,  W.  A.  B.  102,  2b.  534.) 

Lead  telracbloride  with  MCI. 
See  Chloroplumbate,  M. 

Lead  magnesium  chloride,  PbCl2,  2MgCl2  + 
13H2O. 

Deliquescent.  Decomp.  by  H2O.  (Otto 
and  Drewes,  Arch.  Pharm.  228.  495.) 

Lead  potassium  chloride  (potassium  chloro- 
plumbite),  PbCl2,  KC1. 

(Remsen  and  Herty,  Am.  Ch.  J.  14.  125.) 

Contains  Vs  H2O.  (Wells,  Sill.  Am.  J.  145. 
130.) 

See  also  Demassieux,  PbCl2+KCl  under 
PbCl2. 

2PbCl2,  KC1.    (Wells.) 

See  also  Demassieux  as  above. 

Lead  rhodium  chloride. 
See  Chlororhodite,  lead. 

Lead   rubidium    chloride,    PbCl2,    2RbCl+ 


(Wells,  Sill.  Am.  J.  146.  34.) 
2  PbCl2,  RbCl.    (Wells.) 

Lead  sodium  chloride. 
Decomp.  by  H2O. 


Lead  sodium  te/rachloride,  2PbCl4,  9NaCl. 

Very  sol.  in  H2O.  (Sobrero  and  Selmi,  A. 
ch.  (3)  29.  165.) 

See  also  Chloroplumbate,  lead. 

Lead  thallous  chloride,  PbCl2,  3T1C1. 

SI.  sol.  in  cold,  more  in  hot  H2O.  (Noyes, 
Z.  phys.  Ch.  9.  622.) 

PbCl2,  T1C1.  Ppt.  (Ephraim,  Z.  anorg. 
1909,  61.  245.) 

Lead  chloride  ammonia,  2PbCl2,  3NH3. 
(Rose,  Pogg.  20.  157.) 

Lead  te/rachloride  ammonia,  PbCl4,  4NH3. 

Pptd.  from  chloroform  solution.  (Mat- 
thews, J.  Am.  Chem.  Soc.  1898,  20.  825.) 

PbCl4,  2NH3.  Fumes  in  the  air.  Decomp. 
by  H2O.  (Matthews.) 

Lead  chloride  arsenate,  3Pb3(As04)2,  PbCl2. 
See  Arsenate  chloride,  lead. 

Lead    chloride    borate,    Pb(BO2)2,    PbCl2  + 

H2O. 
See  Borate  chloride,  lead. 

Lead  chloride  carbonate. 
See  Carbonate  chloride,  lead. 

Lead  chloride  chlorite. 
See  Chlorite  chloride,  lead. 

Lead  chloride  with  fluoride  and  iodide. 

See  Lead  chlorofluoride  and  Lead  chloro- 
iodide. 

Lead  chloride  phosphate. 
See  Phosphate  chloride,  lead. 

Lead  chloride  phosphite,  PbCl2,  Pb2P2O5(?). 
Ppt.    (Berzelius.) 
Does  not  exist.    (Rose.) 

Lead  chloride  sulphate. 
See  Sulphate  chloride,  lead. 

Lead  chloride  sulphide,  PbCl2,  3PbS. 
See  Lead  chlorosulphide. 

Lead  chlorofluoride,  PbClF. 

SI.  sol.  in  H2O  without  decomp.  Easily 
sol.  in  HNO3+Aq.  (Berzelius.) 

Solubility  in  H2O. 

100  g.  H2O  dissolve  0.0211  g.  PbClF  at 
0°;  0.0370  g.  at  25°;  0.1081  g.  at  100°.  (Starck. 
Z.  anorg.  Ch.  1911,  70.  174.) 

Solubility  in  HCl+Aq  at  25°. 

Solution  of  PbClF  in  HCl+Aq  containing 
0.0535  g.  equiv.  per  1.  contains  0.0758  g. 
PbClF  in  100  cc.  of  solvent. 

Solution  of  PbClF  in  HCl+Aq  containing 


LEAD  HYDROXIDE 


449 


0.1069  g.  equiv.  per  1.  contains  0.1006  g. 
PbCIF  in  100  cc.  of  solvent.  (Starck.) 

Solubility  in  acetic  acid  at  25°. 

Solution"of  PbCIF  in  HC2H3O2  containing 
0.0518  g.  equiv.  per  1.  contains  0.05129  g. 
PbCIF  in  100  cc.  of  solvent. 

Solution  of  PbCIF  in  HC2H3p2  containing 
0.1055  g.  equiv.  per  1.  contains  0.0561  g. 
PbCIF  in  100  cc.  of  solvent.  (Starck.) 

Solubility  in  PbCl2+Aq. 


t 

G.  equiv.  per  1. 
PbCh 

G.  PbCIF  in 
100  cc.  of  solvent 

18° 

0.0100 

0.0020 

u 

0.0195 

0.0016 

u 

0.0495 

0.0002 

25° 

0.00996 

0.0030 

n 

0.0196 

0.0008 

it 

0.0392 

0.0005 

(Starck.) 

Lead  chloroiodide,  2PbCl2,  PbI2. 

Sol.  in  hot  NH4Cl+Aq.  (Poggiale,  J.  pr. 
35.  329.) 

PbCl2,  PbI2.  Sol.  in  hot  HCl+Aq.  (En-, 
gelhardt.) 

Sol.  in  H2O.  (Thomas,  C.  R.  1898,  126. 
1351.) 

Lead  chloroselenide. 

Decomp.  by  boiling  H2O  and  by  cone. 
KOH+Aq.  (Fonzes-Diacon,  C.  R.  1900, 130. 
1133.) 

Lead  chlorosulphide,  PbCl2,  3PbS. 

Partially  decomp.  by  hot  H2O.  Not  at- 
tacked by  dil.,  but  decomp.  by  cone.  HC1  + 
Aq.  (Hunefeld,  J.  pr.  7.  27.) 

PbS,  PbCl2.  Decomp.  by  H2O,  acids,  or 
alkalies.  (Parmentier,  C.  R.  114.  298.) 

ClPbS2PbS2PbS2PbCl.  Ppt.  (Hofmann, 
B.  1904,  37.  250.) 

Lead  fluoride,  PbF2. 

Very  si.  sol.  in  H2O,  and  not  more  in  HF  + 
Aq.  (Berzelius,  Pogg.  1.  31.) 

5.5  millimols  are  sol.  in  1000  ccm.  H2O. 
(Jaeger,  Z.  anorg.  1901,  27.  38.) 

1  1.  HoO  dissolves  640  mg.  at  18°.  (Kohl- 
rausch,  Z.  phys.  Ch.  1904,  50.  356.) 

641  mg.  in  1  1.  of  sat.  solution  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1908,  64.  168.) 

More  sol.  in  HNO3,  or  HCl+Aq.  SI.  sol.  in 
KF+Aq.  (Herty,  Am.  Ch.  J.  14. 107.) 

SI.  sol.  in  dil.  HF+Aq;.  insol.  in  strong 
HF+Aq. 

0.01302  g.  atoms  Pb  are  sol.  in  .1000  cc.  HF. 
(Jaeger,  Z.  anorg.  1901,  27.  37.) 

Insol.  in  liquid  HF.  (Franklin,  Z.  anorg. 
1905,  46.  2.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  J.  Ch. 
1898,  20.  828.) 


Insol.  in  ethylacetate.  (Naumann,  B. 
1910,  43.  314.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329.) 

Lead  potassium  fluoride,  3KF,  HF,  PbF4. 

Decomp.  H2O,  stable  in  dry  air.  (Brauner, 
Z.  anorg.  1894,  7.  7.) 

Lead  silicon  fluoride. 
See  Fluosilicate,  lead. 

Lead  tantalum  fluoride. 
See  Fluotantalate,  lead. 

Lead  titanium  fluoride. 
See  Fluotitanate,  lead. 

Lead  fluoride  sulphate. 
See  Sulphate  fluoride,  lead. 

Lead  hydroxide,  PbO2H2. 

Not  appreciably  sol.  in  H2O.  (Jaeger, 
Z.  anorg.  1901,  27.  38.) 

1  1.  H2O  dissolves  0.155  g.  PbO2H2  at  20° 
and  100°.  (Sehnal,  C.  R.  1909,  148.  1396.) 

Solubility  in  NaOH+Aq. 


G.  Na  in  20  ccm. 


0.2024 
0.3196 
0.5866 
0.9476 
1.7802 


G.  Pb  in  20  ccm. 


0.1012 

0.1736 
0.3532 
0.4071 
0.5170 


(Rubenbauer,  Z.  anorg.  1902,  30.  336.) 
Solubility  of  Pb02H2  in  NaOH+Aq  at  25°. 


G.  mol 

per  1. 

Solid  Phase 

Na 

Pb 

0.274 
0.431 
0.476 
0.745 
1.132 
1.519 

0.0181 
0.287 
0.319 
0.489 
0.711 
0.101 

Pb02H2 

(Wood,  Chem.  Soc.  1910,  97.  884.) 

Insol. -in  acetone.  (Naumann,  B.  1904, 
37.  4329.) 

2PbO,  PbO2H2  =  3PbO,  H2O.  Sol.  in 
10,000  to  12,000  pts.  H2O.  (Yorke.)  Sol.  in 
7000  pts.  H2O.  (v.  Bonsdorff,  Pogg.  41.  307.) 

0.45  millimol.  Pb  are  sol.  in  1  liter  H2O  at 
18°.  (Pleissner,  C.  C.  1907,  II.  1056.) 

Sol.  in  acids.  Insol.  in  NH4OH+Aq.  Sol. 
in  NaOH,  or  KOH+Aq.  Sol.  in  hot  NH4C1+ 
Aq,  and  repptd.  by  NH4OH+Aq. 

Solubility  in  KOH+Aq,  according  to  Ditte 
(C.  R.  94.  130).  When  KOH+Aq  is  gradur 


450 


LEAD  HYDROXIDE 


ally  added  to  lead  hydroxide  suspended  IE 
H2O,  the  lead  hydroxide  is  at  first  dissolved 
proportional  to  the  amount  of  KOH,  until 
the  strength  reaches  200  g.  KOH  to  1  litre 
H2O.  The  solubility  then  diminishes  and 
increases  again  until  400  g.  KOH  are  dis- 
solved in  1  litre  H2O.  The  amorphous  lead 
hydroxide  is  then  converted  into  crystalline 
2PbO(PbO2H2).  By  further  addition  of 
KOH  the  solubility  is  suddenly  decreased, 
and  then  increases  again.  (Ditte.) 

Sol.  in  triethyl  toluenyl  ammonium  hy 
drate+Aq. 

Sol.  in  sorbine+Aq.    (Pelouze.) 
Sol.  in  acetates -fAq.    (Mercer.) 
Sol.  in  Ca,  Ba,  Sr,  K,  or  Na  sucrate+Aq. 
Not  pptd.  in  presence  of  Na  citrate +Aq. 
(Spiller.) 
See  also  under  Lead,  and  Lead  oxide. 


Lead  perhydroxide,  PbO2,  H2O. 
See  Lead  peroxide. 

Lead  imide,  PbNH. 

Decomp.  by  H2O  and  dilute  acids.    (Frank- 
lin, Z.  anorg.  1905,  46.  27.) 


Lead  iodide,  PbI2. 

Sol.  in  187  pts.  boiling  H2O.    (Berthemot.) 

Sol.  in  1235  pts.  H2O  at  ord.  temp.,  and  194 
pts.  at  100°.  (Denot,  J.  pr.  1.  425.) 

Sol.  in  2400  pts.  H2O  at  1S.750.     (Abl.) 

Sat.  PbI2+Aq  at  20°  contains  0.0017  pt.; 
at  27°,  0.002  pt.;  at  100°,  0.0039  pt.  PbI2. 
(Lassaigne,  J.  chim.  med.  7.  364.) 

1 1.  H2O  dissolves  0.6  g.  PbI2  at  10°.  (Ditte, 
C.  R.  92.  718.) 

11.  H2O  dissolves  1.58  millimols  PbI2  at 
25.2°.  (Von  Ende,  Z.  anorg.  1901,  26.  159.) 

0.47  X1CH  gram  are  dissolved  in  1  litre  of 
sat.  solution  at  20°.  (Bsttger,  Z.  phys.  Ch. 
1903,  46.  603.) 


Solubility  in  100  g.  H2O  at  t°. 


HNOs  normal 

s 

0.001 
0.01 
0.051 
0.04    KNO3+ 
0.01    HNO3 

38.87 
39.06 
39.45 

39.45 

t° 

G.  PbI2. 

0 

0.0442 

15 

0.0613 

25 

0.0764  . 

35 

0.1042 

45 

0.1453 

55 

0.1755 

65 

0.2183 

80 

0.3023 

95 

0.3960 

*  100 

0.4360 

*  By  extrapolation. 

(Lichty,  J.  Am.  Chem.  Soc.  1903,  25.  474.) 

0.0013  g.  mol.  PbI2  are  dissolved  in  1  1. 
H2O  at  20°.  (Fedotieff,  Z.  anorg.  1911,  73. 
178.) 

Not  more  sol.  in  HC2H3O2+Aq  than  in 
H2O,  contrary  to  Henry.  (Denot,  I.  c.) 

Pptd.  from  aqueous  solution  by  little  HI+ 
Aq,  but  redissolved  by  the  addition  of  more. 
(Ditte,  C.  R.  92.  718.) 

Insol.  in  cold,  sol.  in  hot  HCl+Aq  with 
decomp. 

Solubility  of  PbI2  in  HN03+Aq  at  25.2°. 
S= Solubility  in  millimols.  per  litre. 


(von  Ende,  Z.  anorg.  1901,  26.  162.) 

Sol.  in  KOH+Aq. 

Sol.  in  cone.  KI,  Nal,  BaI2,  SrI2,  CaI2,  and 
MgI2+Aq,  from  which  it  is  pptd.  by  H2O. 
(Berthemot.) 

Very  sol.  in  KI+Aq,  2  mols.  PbI2  being 
dissolved  for  1  mol.  KI.  (Boullay.) 

Sol.  in  NH4I  + Aq.  Easily  sol.  in  Na2S2O3 + 
Aq.  (Werner,  C.  N.  53.  51.) 

Not  pptd.  in  presence  of  Na  citrate.  (Spil- 
ler.) 

Solubility  in  sat.  I2+Aq  at  20°  =  0.00216  g. 
mol.  per  1.  Solid  phase  PbI2-|-l2.  (Fedotieff, 
Z.  anorg.  1911,  73.  178.) 

Very  easily  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  828.) 

SI.  sol.  in  alcohol.  (Henry.)  Decomp.  by 
boiling  ether.  (Vogel.) 

100  g.  formic  acid  dissolve  0.25  g.  at  19.8°. 
(Aschan,  Ch.  Ztg.  1913,  37.  1117.) 

Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.  257.) 

SI.  sol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1369.) 

Difficultly  sol.  in  methyl  acetate.  (Nau- 
mann, B.  1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Naumann.  B. 
1910,  43.  314.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329.) 

0.02  pts.  are  sol.  in  100  pts.  acetone  at  59°. 

0.02  pts.  are  sol.  in  100  pts.  amyl  alcohol  at 
133.5. 

0.50  pts.  are  sol.  in  100  pts.  aniline  at  13°. 

1.10  pts.  are  sol.  in  100  pts.  aniline  at  184°. 

(Laszczynski,    B.    1894,   27.   2287.) 


LEAD  OXIDE 


451 


Solubility  of  PbI2  in  pyridine  at  t°. 

PbI2,  4KI.     Decomp.   by   H2O;   insol.  in 
alcohol.     (Boullay.)     Does  not  exist.     (R. 

t° 

G.  PbI2  per  100 
g.  pyridine 

Solid  phase 

and  H.) 
3PbI2,    4KI+6H2O.      (Berthelot,    J.    c.) 

Does  not  exist.    (R.  and  H.) 

—37 

0.166 

PbI2,  C5H5N 

—20 

0.175 

u 

Lead  potassium  periodide,  K3Pb2I8+4H2O. 

—  9 
0 
+  3 

0.186 
0.200 
0.215 

a 
U 

Decomp.  by  H2O  or  alcohol.     (Wells,  Z. 
anorg.  4.  346.) 

6 

0.225 

PbI2,  C5H5N  + 
PbI2,  2C5H5N 

Lead  rubidium  iodide,  PbI2,   RbI+2H2O. 

15 

0.208 

PbI2,  2C5H5N 

(Wells,  Sill.  Am.  J.  146.  34.) 

35 

0.188 

' 

57 

0.190 

1 

Lead  silver  iodide,  PbI2,  2AgI. 

77 

0.228 

1 

(Ruff  and  Geisel,  B.   1905,  38.  2663.) 

92 

0.290 

'«,-.'• 

98 
105 

0.340   . 
0.370 

i 

Lead   silver  iodide   ammonia,   PbI2,   2AgI, 
5NH, 

108 

0.410 

t 

OJ-i  -1  JL3* 

112 

0*445 

e 

(Ruff  and  Geisel,   B.   1905,  38.  2663.) 

(Heise,  J.  phys.  Ch.  1912,  16,  273.) 

Lead  hydrogen  iodide,  PbH2I4  =PbI2,  2HI. 

Cold  H2O  dissolves  out  HI.  Sol.  in  hot 
H2O,  from  which  crystallizes  PbI2.  (Guyot, 
J.  chim.  med.  12.  247.) 

+  10H2O.  Decomp.  by  H2O.  (Berthelot, 
C.  R.  91.  1024.) 

Lead  lithium  iodide,  PbI2,  LiI+5H2O. 

Loses  1  mol.  H2O  at  95°  and  loses  another 
mol.  H2O  at  100°.  (Bogorodski,  C.  C.  1894, 
II.  515.) 

PbI2,  2LiI+6H2O.  SI.  sol.  in  H2O.  (Mos- 
nier,  C.  R.  1895,  120.  446.) 

Lead  magnesium  iodide,  PbI2,  2MgI2. 

Decomp.  by  H2O  and  by  alcohol.  (Mos- 
nier,  A.  ch.  1897,  (7)  12.  402.) 

+16H2O.  Very  hygroscopic.  Decomp. 
immediately  by  H2O.  (Otto  and  Drewes, 
Arch.  Pharm.  229.  180.) 

Lead  nickel  iodide,  PbNi2I6+3H2O. 

Decomp.  by  H2O.  (Mosnier,  A.  ch.  1897, 
(7)  12.  411.) 

Lead  potassium  iodide  (Potassium  iodoplum- 
bite),  PbI2,  KI. 

Permanent.  Completely  decomp.  by  H2O. 
Unacted  upon  by  cold,  but  completely  de- 
comp. by  hot  alcohol.  (Boullay,  A.  ch. 
(2)  34.  366.) 

+2H2O.  The  only  salt  that  could  be 
obtained  by  Remsen  and  Herty  (Am.  Ch.  J. 
14.  110.) 

PbI2,  2KI.  SI.  sol.  in  boiling  chloroform; 
easily  sol.  in  strong  KI+Aq,  insol.  in  alcohol. 
(Brooks,  C.  N.  1898,  77.  191.) 

+2H2O.  Decomp.  by  H2O.  (Berthelot, 
A.  ch.  (5)  29.  289.) 

Does  not  exist.    (R.  and  H.) 
.    4-4H2O.    (Ditte,  C.  R.  92.  134.)    Does  not 
exist.    (R.  and  H.) 


Lead  sodium  iodide,  PbI2,  Nal. 

Decomp.  by  H2O.  (Poggiale,  C.  R.  20. 
1180.) 

+zH2O.  (Remsen  and  Herty,  Am.  Ch. 
J.  14.  124.) 

PbI2, 2NaI+6H2O.     SI.   sol.   in    H2O. 
(Moisnier,  C.  R.  1895,  120.  445.) 

Lead  iodide  ammonia,  PbI2,  2NH3, 

Decomp.  by  H2O.  (Rammelsberg,  Pogg. 
48.  166.) 

Lead  iodide  carbonate. 
See  Carbonate  iodide,  lead. 

Lead  iodosulphide,  PbS,  4PbI2. 

Decomp.  by  light,  heat,  acids  and  alkalies. 

(Lenher,  J.  Am.  Chem.  Soc.  1895,  17.  512.) 

Sol.  in  cone.   HI;   insol.   in  dil.   HI+Aq. 

(Lenher,  J.  Am.  Chem.  Soc.  1901,  23.  681.) 

IPbS2PbS2PbI.  Ppt.  (Hofmann,  B.  1904, 
37.  251.) 

Lead  swfroxide,  Pb2O. 

Decomp.  by  H2O  into  PbO2H2. 

Decomp.  by  dil.  H2SO4,  HC1,  HNO3, 
HC2H3O2+Aq,  or  alkalies,  into  PbO,  which 
dissolves,  and  Pb,  which  dissolves  or  not, 
according  to  the  reagent.  Sol.  in  dil. 
Pb(N03)2+Aq. 

Lead  monoxide  (Litharge),  PbO. 

Sol.  in  7000  pts.  H2O.     (Horsford.) 

Pure  PbO  is  insol.  in  H2O.  (Brandecke, 
Repert.  53.  155;  Siebold,  Repert,  63.  174; 
Herbergen,  Repert.  66.  55.)  SI.  sol.  in  H2O. 
(Yorke,  Phil.  Mag.  (3)  6.  82.) 

0.31  millimoles  Pb  are  dissolved  in  1  liter 
H2O  at  18°.  (Pleissner,  C.  C.  1907,  II.  1056.) 

1.71  X10-2  g.  are  dissolved  in  1  litre  of  sat. 
solution  at  20°.  (Bottger,  Z.  phys.  Ch.  1903, 
46.  603.) 

Easily  sol.  in  acids. 


452 


LEAD  OXIDE 


Sol.  in  KOH,  or  NaOH+Aq;  also  in 
CaO2H2+Aq. 

Sol.  in  boiling  Cu(NO3)2+Aq  with  pptn.  of 

Sol.  in  CaCl2,  and  SrCl2+Aq.  (Andre, 
C.  R.  104.  359.) 

Sol.  in  MgCl2+Aq.  (Voigt,  Ch.  Ztg.  13. 
695.) 

Sol.  in  boiling  Cu(NO3)2+Aq  with  pptn.  of 
CuO. 

Partially  sol.  in  Cd(NO3)2,  and  Mn(NO3)2 
+Aq  with  pptn.  of  CdO  and  MnO  respec- 
tively. 

Not  acted  upon  by  Mg,  Ag,  Co,  Ni,  or  Ce 
nitrates  +  Aq.  (Persoz.) 

Very  sol.  in  Pb(C2H3O2)2+Aq.  (Rochle- 
der.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1883, 
II,  1014.) 

When  finely  pulverised,  sol.  in  cane  sugar 
+Aq,  but  less  than  Pb3O4.  (Peschier.) 

SI.  sol.  in  glycerine.  Readily  sol.  in  glucose 
+Aq.  (Persoz.) 

Sol.  in  volatile  oils.     (Schweitzer.) 

Yellow  modification. 

Solubility  in  H2O  at  22°. 


Solubility  in  g.- 
equiv.  per  litre 

1.  Yellow  PbO,  obtained  by 
boiling  lead  hydroxide 
with  10%  NaOH 
2.  Yellow  PbO,  obtained  by 
heating  1  at  630° 
3.  Yellow  PbO,  obtained  by 
heating  at  740°  red  PbO, 
formed  by  boiling  lead 
hydroxide    with    cone. 
NaOH 
4.  Yellow  PbO  obtained  by 
heating  pure,  commer- 
cial, yellow-brown  PbO 
at  620°. 

1.03  x  10-4 

l.OSxlO-4 
l.OOxlO-4 

1.09xlO-4 

(Ruer,  Z.  anorg.  1906,  60.  273.) 

Red  modification.  Obtained  by  boiling 
lead  hydroxide  with  cone.  NaOH+Aq. 

Solubility  in  H2O  at  22°  =  0.56X10-4  g. 
equiv.  per  1.  (Ruer,  Z.  anorg.  1906,  50.  273.) 

Yellow-brown  modification.  Solubility  in 
H2O  at  22°  =  1.10X10-4  g.  equiv.  per  litre. 
(Ruer,  Z.  anorg.  1906,  60.  273.) 

See  also  Lead. 

Min.  Massicot. 

Lead  oxide  (Red  lead),  Pb3O4. 

Insol.  in  H2O. 

Converted  by  acids  into  PbO2  and  salts  of 
monoxide. 

Sol.  in  a  large  amt.  of  glacial  acetic  acid. 
(Berzelius.)  Insol.  in  acetic  acid.  (Schon- 
bein,  J.  pr.  74.  325.) 


Solution  in  HC2H3O2+Aq  may  decompose 
or  not  according  to  concentration  of  acid. 
When  treated  with  an  excess  of  HC2H3O2+ 
Aq  of  8°  B,  Pb3O4  is  quickly  dissolved,  but 
the  solution  soon  deposits  PbO2;  this  de- 
composition is  facilitated  by  dilution.  But 
if  Pb3O4  is  treated  with  a  large  excess  of 
glacial  HC2H3O2,  it  dissolves,  and  the  solu- 
tion is  permanent  if  atmospheric  air  is  ex- 
cluded, and  temp,  does  not  rise  above  40°. 
(Jacquelain,  J.  pr.  63.  152.) 

Insol  in  acetone.  (Eidmann,  C.  C.  1899, 
II,  1014;  Naumann,  B.  1904,  37.  4329.) 

Easily  sol.  in  cane  sugar +Aq.    (Peschier.) 

Min.  Minium. 

Lead  sesquioxide,  Pb2O3. 

Insol.  in  H2O  or  in  KOH+Aq. 

Decomp.  by  strong  acids  into  PbO2  and 
corresponding  salt  of  monoxide. 

Lead  peroxide,  PbO2. 

Insol.  in  H2O.  Sol.  in  acids,  also  in  cone, 
alkali  hydroxides +Aq.  The  solutions  in 
acids  are  very  unstable,  except  when  con- 
centrated and  kept  at  a  low  temperature. 

Decomp.  by  cold  HC1,  HCN,  HBr,  and 
HI+  Aq.  Not  attacked  by  other  acids  when 
cold,  but  decomp.  thereby  when  hot.  Insol. 
in  moderately  cone.  HNO3,  H2SO4,  or 
HC2H3O2+Aq. 

There  are  two  forms  of  PbO2,  the  amor- 
phous and  the  crystalline. 

1  1.  of  very  cone.  H2SO4  dissolves  10  milli- 
mols.  crystalline  PbO2. 

Solubility  of  amorphous  PbO2  in  H2SO4+Aq 
at  22°. 

99.5  millimols.  PbO2  are  dissolved  in  1  1.  of 
acid  containing  1720  g.  H2SO4. 

4  millimols.  PbO2  are  dissolved  in  1  1.  of 
acid  containing  1097  g.  H2SO4. 

v  =  moles  H2SO4  per  mole  of  H2O. 

c=  millimols.  PbO2  dissolved  in  1  litre. 


0.32 
0.30 
0.25 


0.82 

0.4 

7.10-2 


0.20 
0.15 
0.10 


8.10-3 
5.10-4 
1.10-5 


(Dolezalek  and  Finckli,  Z.  anorg.   1906,  51. 
323-5.) 

Decomp.  by  NH4OH+Aq.  Sol.  in  cone. 
KOH,  or  NaOH+Aq. 

Sol.  with  decomp.  in  Hg2(NO3)2+Aq. 
(Levol.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II,  1014;  Naumann,  B.  1904,  37.  2943.) 

Min.  Plattnerite. 

Lead  manganese  peroxide,  PbO2,  4MnO2. 

Ppt.  (Gibbs  and  Parkmann,  Sill.  Am.  J. 
(2)  39.  58.) 


LEAD  SULPHIDE  MERCURIC  CHLORIDE 


453 


Lead  oxybromide,  PbBr2,  PbO. 

Insol.  in  H2O. 

+1,  IY2,  and  3H2O.  (Andre,  C.  R.  96. 
1502.) 

6PbO,  PbBr2+2H2O.  Ppt.  (Stromholm, 
Z.  anorg.  1904,  38.  436.) 

Lead  oxychloride,  2PbCl2,  PbO+2H2O. 

(Andre,  C.  R.  96.  435.) 

PbCl2,  PbO.  Absolutely  insol.  in  hot  or 
cold  H2O.  (Andre,  A.  ch.  (6)  3.  108.) 

Min.  Matlockile. 

+H2O.    Sol.  in  hot  NaOH+Aq.    (Andre.) 

0.38  miliimols.  Pb  are  dissolved  in  1  litre 
H2O  at  18°.  (Pleissner,  C.  C.  1907,  II.  1055.) 

PbCl2,  2PbO.  Insol.  in  H2O.  Sol.  in  dil. 
KOH  + Aq  (about  1 10  g.  in  1 1.)  (Ditte,  C.  R. 
94.  1180.) 

Min.  Mendipite.    Easily  sol.  in  HNO3  + Aq. 

+2H2O.    (Andre,  A.  ch.  (6)  3.  111.) 

PbCl2,  3PbO.  Insol.  in  H2O.  (Dober- 
einer.) 

+  i^H2O.  Ppt.  (Stromholm,  Z.  anorg. 
1904,  38.  435.) 

+2H2O.  0.10  miliimols.  Pb  are  dissolved 
in  1  litre  H2O  at  18°.  (Pleissner,  C.  C.  1907, 
II.  1056.) 

+3H2O.    Ppt.    (Andre,  C.  R.  104.  359.) 

+4H2O.  Nearly  insol.  in  H2O.  SI.  sol. 
in  NaOH+Aq.  (Vauquelin.) 

PbCl2,  5PbO.    (Dobereiner.) 

6PbO,  PbCl2+2H2O.  Ppt.  (Stromholm, 
Z.  anorg.  1904,  38.  434.) 

PbCl2,  7PbO.     Cassel-yellow. 

Lead  strontium  oxychloride,  2PbO,  SrCl2  + 

5H20. 
(Andre,  C.  R.  104.  359.) 

Lead  oxychloride,  iodide,  PbCl2,  PbI2,  4PbO. 
Min.     Schwartzenbergite.       Sol.     in     dil. 
HN03+Aq. 

Lead  oxyiodide,  PbI2,  PbO. 

Insol.  in  boiling  H2O  or  KI  +  Aq .  (Brandes, 
A.  10.  269.) 

+  3/£H2O.    (Ditte,  C.  R.  92.  145.) 

+H20. 

PbI2,  2PbO.  Insol.  in  H2O.  (Denot,  J. 
Pharm.  20.  1.) 

+H20.    . 

PbI2,  3PbO+2H2O.  Ppt.  (Kiihn,  C.  C. 
1847.  593.) 

PbI2,  5PbO.     Insol.  in  H2O.     (Denot.) 

+7H2O.    (Ditte,  C.  R.  92.  145.) 

6PbO,  PbI2+2H2O.  Ppt.  (Stromholm, 
Z.  anorg.  1904,  38.  437.) 

9PbO,  PbI2  +2H2O.  (Stromholm,  Z.  anorg. 
1904,  38.  437.) 

Lead  oxyperiodide,  PbO,  PbI2I3. 

Decomp.  by  boiling  H2O.  Sol.  in  dil. 
HC2H3O2+Aq.  (Groger,  W.  A.  B.  100,  2b. 
415.) 


Lead  phosphide,  PbP6. 

Decomp.  by  H2O  and  dil.  acids.  (Bossuet, 
C.  R.  1913,  167.  721.) 

Lead  phosphoselenide,  PbSe,  P2Se. 

Insol.inH2OorHCl+Aq.  Sol.inHNO3+ 
Aq. 

Insol.  in  cold,  slowly  decomp.  by  hot  al- 
kalies+Aq.  (Hahn,  J.  pr.  (2)  93.  436.) 

2PbSe,  P2Se3.  Insol.  in  H2O,  HC1,  or 
HNO3+Aq.  Slowly  sol.  in  red  fuming 
HN03.  (Hahn.) 

2PbSe,  P2Se5.  Decomp.  by  fuming  HNO3. 
(Hahn.) 

Lead  selenide,  PbSe. 

Cold  HNO3+Aq  dissolves  Pb  with  separa- 
tion of  Se,  which  dissolves  on  warming. 
(Little,  A.  112.  212.) 

Min.  Clausthalite.  Sol.  in  HNO3+Aq 
with  separation  of  Se,  when  warmed. 

Lead  mercury  selenide,  (Pb,  Hg)Se. 
Min.  Lehrbachite. 

Lead  sulphide,  PbS. 

Very  si.  sol.  in  H2O. 

1  1.  H2O  dissolves  3.6  X10-5  moles.  PbS  at 
18°.  (Weigel,  Z.  phys.  Ch.  1907,  68.  294.) 

1  1.  H2O  dissolves  3X10-4  g.  PbS  at  25°. 
(Hevesy,  Z.  anorg.  1913,  82.  328.) 

Insol.  in  dilute  acids;  alkalies,  and  alkali 
sulphides  +Aq.  Decomp.  with  solution  in 
moderately  dil.  HNO3+Aq.  With  cone. 
HNO3  or  aqua  regia,  PbSO4  is  formed.  Sol. 
in  hot  cone.  HCl+Aq. 

1 1.  H2O  sat.  with  H2S  dissolves  1.5  X10-4  g. 
PbS  at  25°.  (Hevesy,  Z.  anorg.  1913,  82. 
328.) 

Insol.  in  NH4C1,  or  NH4NO3  +  Aq.    (Brett.) 

Somewhat  sol.  in  H2S+Aq  when  heated 
therewith  in  a  sealed  tube.  (Senarmont,  A. 
ch.  (3)  32.  168.) 

Insol.  in  potassium  thiocarbonate  +Aq. 
(Rosenbladt,  Z.  anal.  26.  15.) 

Sol.  in  Na2S2O3+Aq.  (Waller,  J.  Anal. 
Ch.  5.  646.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

Min.  Galena,  Galenite. 

Lead  pofo/sulphide,  PbS5. 

Ppt.;  insol.  in  alkali  sulphides;  decomp. 
by  cone.  HNO3.  (Bodroux,  C.  R.  1900,  130. 
1398.) 

Lead  platinum  sulphide. 
See  Sulphoplatinate,  lead. 

Lead    sulphide    mercuric    chloride,    3PbS. 

4HgCl2. 

Decomp.  by  H2O.  (Levallois,  C.  R.  96. 
1666.) 


454 


LEAD  SULPHOBROMIDE 


Lead  sulphobromide,  chloride,  or  iodide. 
See  Lead  bromosulphide,  etc. 


Lead  cfosulphocMmide,  PbN2S2,  NH3. 

Ppt. 

Very  stable  in  the  air  or  in  a  vacuum. 

Sol.  in  no  solvent  without  decomp. 

When    rapidly    heated  •  it    explodes    very 
violently  at  140°.    (Ruff,  B.  1904,  37. 1581.) 


Lead  telluride,  PbTe. 

Insol.  in  H2O.  Sol.  in  cold  HNO3+Aq. 
(Rose,  Pogg.  18.  68.) 

Min.  Altaite.     Easily  sol.  in  HNO3+Aq. 

"  Leucone." 

Wohler  (A.  127.  268)  gives  this  substance 
the  formula  HioSisOjo,  but  it  is  identical  with 
silicoformic  anhydride,  Si2H2O3,  which  see. 

Lime. 

Quicklime,  CaO.    See  Calcium  oxide. 
Slaked   lime,   CaO2H2.     See  Calcium  hy- 
droxide. 

Lithium,  Li. 

Decomposes  H2O. 

Easily  sol.  in  dil.  acids.    Slowly  attacked  by 
cone.  H2SO4,  rapidly  by  cone.  HNO3+Aq. 
Insol.  in  hydrocarbons.    Sol.  in  liquid  NH3, 
but  not  so  easily  as  K. 

Sol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  820.) 

1  gram  atom  dissolves: 
at         0°  in  3.93  mol.  liquid  NH3. 
«   — 25°    "  3.93       "          "          " 
«   — 50°    "  3.93       «         ."          " 
«   — 80°    "  3.93       "          "          " 
(Ruff,  B.  1906,  39.  840.) 

Sol.  in  ethylamine.  Insol.  in  propylamine 
and  in  secondary  and  tertiary  amines.  (Kraus, 
J.  Am.  Chem.  Soc.  1907,  29.  1561.) 

Lithium  amalgam,  LiHg5. 

LiHgs  is  obtained  at  all  temp,  up  to  100°. 
Can  be  cryst.  from  Hg  without  decomp.  at 
any  temp,  below  100°.  (Kerp,  Z.  anorg.  1900, 
25.  68.) 

Lithium  amide,  LiNH2. 

(Ruff,  B.  1911,44.505.) 

Decomp.  slowly  in  the  air. 

Slowly  decomp.  by  cold,  rapidly  by  hot 
H2O. 

Slowly  decomp.  by  HC1. 
.     Slowly  decomp.  by  cold,  rapidly  by  hot 
abs.  alcohol.     (Titherley,  Chem.  Soc.  1894, 
66.  518.) 

Tnlithium  amide,  Li3NH2. 

Hydroscopic;  decomp,  by  H2O,  (Dafert, 
M.  1910,  31.  994.) 


Lithium  ammonia,  Li,  NH3. 

Decomp.  by  H2O  at  ordinary  temp.;  sol. 
in  liquid  NH3.  (Moissan,  C.  R.  1898,  127. 
689.) 

Li,  3NH3.    (Moissan,  C.  R.  1901, 133.  716.) 

Tnlithium  ammonium,  Li3NH4. 

Very  hydroscopic,  decomp.  by  H2O.  (Da- 
fert, M.  1910,  31.  992.) 

Lithium  antimonide,  Li3Sb. 

Decomp.  by  H2O  with  evolution  of  H2. 
Sol.  in  liquid  NH3.  (Lebeau,  C.  R.  1902,  134. 

285.) 

Lithium  arsenide,  Li3As. 

Decomp.  by  H2O;  decomp.  violently  by 
fuming  HNO3.  (Lebeau,  C.  R.  1899, 129.  50.) 

Lithium  azoimide,  LiN3. 

Deliquescent.    Stable  in  aq.  solution. 

36.12  pts.  are  sol.  in  100  pts.  H2O  at  10°. 

62.07     "    "     "     "  100    "    H2O   "  15.5°. 

66.41     "    "     "     "  100    "    H2O    "  16°. 

20.26  "  "  "  "  100  "  abs.  alcohol 
at  16°. 

Insol.  in  ether.  (Curtius,  J.  pr.  1898,  (2) 
68.  277.) 

+H2O.  Very  hydroscopic;  decomp.  in  the 
air.  Very  sol.  in  H2O  and  alcohol.  (Dennis, 
Z.  anorg.  1898, 17.  18.) 

Lithium  bromide,  LiBr. 
Deliquescent. 
100  pts.  H2O  dissolve  at: 
0°       34°       59°       82°   '    103° 
143      196      222      244      270  pts.  LiBr. 

Sp.  gr.  of  LiBr+Aq  at  19.5°  containing: 
0          10        15        20        25       30%  LiBr, 
1.035   1.072   1.113   1.156   1.204  1.254 

35        40        45        50       55%  LiBr. 
1.309   1.368   1.432   1.500   1.580 
(Kremers,  Pogg.  103.  65;  104.  133:  Gerlach, 
Z.  anal.  8.  285.) 

Temp,  of  maximum      g.-mol.  LiBr  dissolved 

density  of  LiBr+Aq.          in  1000  g.  H2O. 

1.921°  0.2941 

0.881°  0.4383 

(de  Coppet,  C.  R.  1900,  131.  178.) 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  828.) 

Sol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1369.) 

Solubility  in  glycol  at  14.7°  =  37.5%.  (de 
Coninck,  Belg.  Acad.  Bull.  1905,  359.)  - 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328;  Eidmann,  C.  C.  1899,  II.  1014.) 

Sol.  in  methyl  acetate  (Naumann,  B.  1909, 
42.  3789) ;  ethyl  acetate.  (Naumann,  B.  1904, 
37.  3601.) 


LITHIUM  CHLORIDE 


455 


Difficultly  sol.  in  ethyl  acetate.  (Nau 
mann,  B.  1910,  43.  314.) 

+H2O.  100  g.  H2O  dissolve  209  g.  LiB 
at  44°.  (Bogorodski,  C.  C.  1894,  II.  514.) 

+2H2O.    (Bogorodski.) 

+3H2O.  100  g.  H2O  dissolve  80  g.  LiB 
at  —30°,  and  122  g.  at  —10°.  (Bogorodski 

Lithium  molybdenyl  bromide,  LiBr,  MoOBr 

+4H20. 

Very  hygroscopic.  (Weinland  and  Knoll 
Z.  anorg.  1905,  44.  111.) 

Lithium  bromide  ammonia. 

LiBr,  NH3.    Sol.  in  H2O  with  decomp. 
LiBr,  2NH3.    "     "      "      " 
LiBr,  3NH3.    "     "      "      " 
LiBr,  4NH3.    "    "      "      "          " 
(Bonnefoi,  C.  R.  1900,  130.  1395.) 

Lithium  carbide,  LiC2. 

Insol.  in  cone,  acids. 

Sol.  in  fused  oxidizing  agents;  decomp.  H20 
in  the  cold.  (Moissan,  C.  R.  1896,  122.  363.) 

Lithium  sw&chloride,  Li2Cl. 

Decomp.  by  H2O.  (Guntz,  C.  R.  1895, 
121.  945.) 


Lithium  chloride,  LiCl. 

Very  deliquescent.  Most  deliquescent  salt 
known  to  Berzelius.  Very  sol.  in  H2O.  Sol. 
in  1.315  pts.  H2O  at  15°.  (Gerlach.) 

100  pts.  H2O  dissolve  at: 
0°     20°      65°    80°   69°   140°  160° 
63.7  80.7  104.2  115  129  139   145  pts.  LiCl. 
(Gerlach,  Z.  anal.  8.  281.) 

Sp.  gr.  of  LjCl+Aq  at  15°  containing: 
1  5  10  15          20%  LiCl, 

1.006      1.030      1.058      1.086       1.117 

25  30  35          40%  LiCl. 

1.148      1.182      1.219      1.256 
(Gerlach,  Z.  anal.  8.  281.) 

Sp.  gr.  of  LiCl+Aq  at  18°  containing: 

5  10          20         30          40%  LiCl. 

1.0274      1.0563     1.115     1.181      1.255 

(Kohlrausch,  W.  Ann.  1879.  1.) 

Sp.  gr.  of  LiCl+Aq  at  25°. 


Sp.  gr.  of  LiCl+Aq. 

g.  LiCl  in  1000  g. 
of  solution 

Sp.  gr.  1(B°/16° 

0 

2.3923 
6.2360 
10.1093 

1.000000 
1.001405 
1.003647 
1.005921 

Concentration  of  LiCl+Aq. 

Sp.  gr. 

1-normal 

Vr-       " 
l/«-       " 

Vr-       " 

1.0243 
1.0129 
1.0062 
1.0030 

Normality  of 
LiCl  +Aq 

%  LiCl 

Sp.  gr. 

10.35 
7.17 
5.57 
2.98 
1.06 

35.97 
26.40 
21.10 
11.83 
4.37 

•1.2230 
1.1550 
1.1215 
1.0691 
1.0232 

(Wagner,  Z.  phys.  Ch.  1890,  6.  38.) 


(Dijken,  Z.  phys.  Ch.  1897,  24.  109.) 

Sp.  gr.  of  LiCl-hAq  at  0°. 
%LiCl  4.26   12.18   22.2    32.5    41.4    43.2 
Sp.  gr.    1.026  1.073  1.133  1.203  1.267  1.282 
(Lemoine,  C.  R.  1897,  125.  603.) 

Sp.  gr.  of  LiCl+Aq  at  20°. 


(Forchheimer,  Z.  phys.  Ch.  1900,  34.  25.) 


Sp.  gr.  20°/4°  of  a  normal  solution  of  LiCl  = 
1.022375.  (Haigh,  J.  Am.  Chem.  Soc.  1912, 
34.  1151.) 


Sp.  gr.  of  dil.  LiCl+Aq  at  20.004°. 
Conc.  =  g.  equiv.  LiCl  per  1.  at  20.004°. 
Sp.  gr.  compared  with  H2O  at  20.004  =  1. 


Cone. 

Sp.  gr. 

0.0000 

.000,000,0 

0.0001 

.000,002,5 

0.0002 

.000,005,0 

0.0005 

.000,012,6 

0.0010 

:  .000,025,3 

0.0020 
0.0050 

.000,050,5 
.000,125,8 

-  -0.0100 

.000,251,0 

Lamb  and  Lee,  J.  Am.  Chem.  Soc.  1913,  36. 
1688.) 


B.-pt.  of  LiCl+Aq. 


%  LiCl 

B.-pt. 

%  LiCl 

B.-pt 

3.38 
6.54 
13.04 

101° 
102 
105 

16.66 
19.35 
21.8 

107° 
109 
111 

(Skinner,  Chem.  Soc.  61.  341.) 

456 


LITHIUM  CHLORIDE 


Sat.  LiCl+Aq  boils  at  171°.  (Kremers.) 

B.-pt.  of  LiCl+Aq.  P  =pts.  LiCl  to 
100  pts.  H2O. 


B.-pt. 


101° 

102 

103 

104 

105 

106 

107 

108 

109 

110 

111 

112 

113 

114 

115 

116 

117 

118 

119 

120 

121 

122 

123 


3.5 

7 
10 
12.5 
15 

17.5 
20 
22 
24 
26 
28 
30 
32 
33.5 
35 
36.5 
38 

39.5 
41 

42.5 
44 
45.5 
47 


B.-pt. 


124° 

125 

126 

127 

128 

129 

130 

131 

132 

133 

134 

135 

136 

137 

138 

139 

140 

141 

142 

143 

144 

145 

146 


48.5 

50 

51.5 

53 

54.5 

56 

57.5 

59 

60.5 

62 

63.5 

65 

66.5 

68 

69.75 

71.5 

73.25 

75 

77 

79 

81 

83 

85 


B.-pt. 


147° 

148 

149 

150 

151 

152 

153 

154 

155 

156 

157 

158 

158.5 

159 

160 

161 

162 

163 

164 

165 

166 

167 

168 


87.5 

90 

92.5 

95 

97.5 
100 
102.5 
105 
107.5 
110.5 
113.5 
116.5 
117.96 
119.5 
122.5 
125.5 
128.5 
131.5 
135 
138.5 
142.5 
146.5 
151 


(Gerlach,  Z.  anal.  26.  437.) 
Solubility  of  LiCl  in  HCl+Aq  at  0°. 


Mg.  mol.  per  10  cc. 
of  solution 


LiCl 


120 
97.5 
67.0 
58.0 


HCl 


0.0 
22.5 
66.0 
81.0 


G.  per  10  cc.  of 
solution 


LiCl 


51.0 
41.4 

28.5 
24.6 


HCl 


0.0 

8.2 

24.1 

29.5 


Sp.  gr.  of 
solution 


1.255 
1.243 
1.249 
1.251 


(Engel,  A.  ch.  (6)  13.  385.) 

See  also  LiCl+H2O. 

SI.  sol.  in  liquid  NH3.    (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

Sol.  in  absolute  alcohol,  ether,  and  alcohol- 
ether. 

B.-pt.  of  alcoholic  solution  of  LiCl. 


%  LiCl 


2.4 

5.39 

8.01 


B.-pt. 


78. 43° +0.70° 
"      +2.15 

"      +4.18 


%  LiCl 


9.93 
15.94 


B.-pt. 


78.43°+  5.55° 
"     +11.75 


(Skinner.) 

Solubility  in  alcohol +Aq  decreases  to  40% 
alcohol +60%  H2O.  Curve  shows  minimum 
at  30%  H2O  to  70%  alcohol.  The  sat.  pure 
H2O  and  pure  alcohol  solutions  cooled  to  0° 
deposit  LiCl,  H2O  and  LiCl,  4C2H6O  respec- 
tively. (Pina  de  Rubies,  C.  A.  1914.  743 
3006.) 


Solubility  in  ethyl  alcohol. 

Temp.       1.06°  5.07°  13.0°  25.0°  40.6°  62.6° 

%  LiCl       14       14       13       14       15       18 

(Lemoine,  C.  R.  1897,  125.  605.) 

100  g.  ethyl  alcohol  dissolve  at: 
0°  5°         10°        15°          17° 

14.42      15.04     16.77     18.79      20.31  g.  LiCl. 
The  solid  phase  from  0°-17°  is  LiCl,  4C2H6O 

20°         30°        40°        50°         60° 
24.28      25.10    25.38    24.40    23.46  g.  LiCl. 
The   solid   phase   from   20°-60°   is   LiCl. 
(Turner  and  Bissett,  Chem.  Soc.  1913,   103 
1907.) 


Solubility  in  ethyl  alcohol +Aq  at  25°.. 


100  g.  of  the  solution  contain 


G.  C2H5OH 


0 

5.96 
11.07 
17.46 
18.56 
22.16 
26.29 
28.97 
29.27 
30.10 
30.51 
32.79 
38.40 
49.27 
50.32 
53.50 
58.15 
59.78 
63.09 
70.24 
70.70 
70.74 
79.26 


G.  H2o 


55.10 
51.52 
48.73 
43.90 
43.70 
41.17 
39.51 
37.42 
36.89 
36.64 
35.67 
34.95 
31.58 
24.67 
24.04 
20.94 
18.47 
17.46 
14.83 
8.66 
8.26 
7.78 
0 


G.  LiCl 


44.90 
42.52 
40.20 
38.64 
37.74 
36.67 
34.70 
33.61 
33.84 
33.26 
33.82 
32.26 
30.02 
26.06 
25.64 
25.56 
23.38 
22.76 
22.08 
21.10 
21.04 
21.48 
20.74 


The  solid  phase  in  the  mixtures  which  are 
richest  in  alcohol  is  LiCl;  in  the  other  mix- 
tures the  solid  phase  is  LiCl+H2O. 

(Pina  de  Rubies,  C.  C.  1915,  I.  521.) 


Sp.   gr.   of  LiCl  in   ethyl  alcohol   (LiCl, 
2C2H60). 


%  salt 

Sp.  gr.  at  14° 

Sp.  gr.  at  0° 

0 
5.2 
10.1 
14.6 

0.797 
0.839 
0.871 
0.903 

0.809 
0.851 
0.881 
0.903 

(Lemoine,  C.  R.  1897,  125.  605.) 


LITHIUM  URANIUM  CHLORIDE 


457 


Solubility  in  methyl  alcohol  at  t°. 

Solubility  of  LiCl  in  acetone. 

t° 

%  LiCl  in  sat.  solution 

Pts.  sol.  in  100  pts.  acetone 

t° 

1 
23 
50 

26 
27 
30 

4.60 
4.40 
4.11 
3.76 
3.12 
2.14 

0 
12 
25 
46 
53 
58 

(Lemoine,  C.  R.  1897,  125.  604.) 

Sp.  gr.  of  LiCl  in  methyl  alcohol  (LiCl, 
3CH40). 

(Laszczynski,  B.  1894,  27.  2287.) 

%salt  5.2  14.5  22.1 

Sp.  gr.  at  21.5°   0.836          0.910          0.974 
Sp.  gr.   "  0°         0.854          0.926          0.988 
(Lemoine,  C.  R.  1897,  126.  604.) 

15.86  g.  are  sol.  in  100  g.  propyl  alcohol. 
(Schlamp,  Z.  phys.  Ch.  1894,  14.  276.) 

Sol.  in  15  pts.  fusel  oil.    (Gooch,  Am.  Ch.  J. 
9.  33.) 

100  g.  methyl  alcohol  dissolve  42.36  g.  LiCl 
at  25°. 

100  g.  ethyl  alcohol  dissolve  25.83  g.  LiCl 
at  25°. 

.     100  g.  propyl  alcohol  dissolve  16.22  g.  LiCl 
at  25°. 

100  g.  isoamyl  alcohol  dissolve  9.03  g.  LiCl 
at  25°. 

(Turner  and  Bissett,  Chem.  Soc.  1913,  103. 
1909.) 

Solubility  of  fused  LiCl  in  alcohols  at  25°. 


(Patten  and  Mott,  J.  phys.  Chem.  1904,  8. 

158.) 

100  pts.  pyridine  dissolve  7.78  pts.  LiCl  at 
15°;  14.26  pts.  LiCl  at  100°.  (Laszczynski, 
B.  1894,  27.  2288.) 

Soluble  in  anhydrous  pyridine,  97%  pyri- 
dine+Aq,  95%  pyridine +Aq,  and  93% 
pyridine +Aq.  (Kahlenberg,  J.  Am.  Chem. 
Soc.  1908,  30.  1107.) 

Difficultly  sol.  in  methyl  acetate  (Nau- 
mann,  B.  1909,  42.  3789);  ethyl  acetate. 
(Naumann,  B.  1910,  43.  314.) 

Sol.  in  ethyl  acetate.  (Naumann,  B.  1904, 
37.  3601.) 

Solubility  in  glycol  at  15°  =  11%.  (de 
Coninck,  Belg.  Acad.  Bull.  1905,  359.) 

Insol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1370.) 

Sol.  in  ethylamine.  (Shinn.  J.  phys.  Chem. 
1907,  11.  538.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899,  II. 
1014.) 


+H2O.  13.536  millimols.  are  contained 
in  1  1.  sat.  solution  at  25°.  (Herz,  Z.  anorg. 
1912,  73.  274.) 

Solubility  in  HCl+Aq  at  25°. 


Millimols  HC1  in  10  ccm. 

Millimols  LiCl  in  10  ccm. 

6'.30 
10.53 
17.64 

135.36 
134.14 
126.52 
122.58 

Solvent 

%  LiCl 

Water 
Ethyl  alcohol 
Propyl  alcohol 
Butyl  alcohol 
Amyl  alcohol 
Allyl  alcohol 
Glycerine 
Phenol  (at  53°C) 

45.0 
2.475 
3.720 
9.56 
8.26 
4.20 
4.14 
1.89 

(Herz,  Z.  anorg.  1912,  73.  274.) 

+2H2O.  Sol.  in  acetone.  (Krug  and 
M'Elroy,  J.  Anal.  Ch.  6.  184.) 

+3H2O.  (Bogorodski,  C.  C.  1894,  II. 
514.) 

Lithium  gold  chloride. 
See  Chloraurate,  lithium. 

Lithium  manganous  chloride,  LiCl,  MnCl2  + 

3H2O. 

Decomp.  by  H2O;  stable  only  in  excess  of 
LiCl.  (Chassevant,  A.  ch.  (6)  30.  10.) 

Lithium  mercuric  chloride,  2LiCl,  HgCl2. 

Very  deliquescent  and  sol.  in  H2O.  (Harth, 
Z.  anorg.  1897,  14.  323.) 

Lithium  nickel  chloride,  LiCl,  NiCl2+3H2O. 
Deliquescent.     Sol.  in  H2O  and  alcohol. 
(Chassevant.) 

Lithium    thallic    chloride,    SLiCl,    T1C13  + 

8H2O. 

Very  deliquescent.  Sol.  in  H2O.  (Pratt, 
Am.  J.  Sci.  1895,  (3)  49.  404.) 

Lithium  stannic  chloride. 
See  Chlorostannate,  lithium. 

Lithium  uranous  chloride,  Li2UCl6. 

As  K  salt.  (Aloy,  Bull.  Soc.  1899,  (3)  21. 
264.) 

Lithium  uranium  chloride,  UC14,  2LiCl. 

Very  hydroscopic;  sol.  in  H2O  with  decomp. 
Sol.  in  acetic  acid.  Decomp.  by  alcohol. 
(Aloy,  Bull.  Soc.  1899,  (3)  21.  264.) 


458 


LITHIUM  ZINC  CHLORIDE 


Lithium  zinc  chloride,  LiCl,  ZnCl2+3H20. 

Extremely  deliquescent.  (Ephraim,  Z. 
anorg.  1908,  69.  68.) 

3LiCl,  ZnCl2+10H2O  (?).  Not  obtained 
in  solid  state.  (Ephraim,  Z.  anorg.  1908,  69. 
69.) 

Lithium  chloride  ammonia. 

LiCl,  NH3. 

LiCl,  2NH3.  ' 

LiCl,  3NH3. 

LiCl,  4NH3. 

Above  salts  are  all  decomp.  by  H2O. 
(Bonnefoi,  C.  R.  1898,  127.  367-369.) 

Lithium  chloroiodide,  LiCl4I+4H2O. 

Deliquescent.  (Wells  and  Wheeler,  Sill. 
Am.  J.  144.  42.) 

Lithium  fluoride,  LiF. 

Very  difficultly  sol.  in  H2O.  (Berzelius, 
Pogg.  1.  17.) 

Two  crystalline  forms.  Only  very  si.  sol. 
in  H2O.  Very  si.  decomp.  by  H2O  at  red 
heat.  (Poulenc,  Bull.  Soc.  1894,  (3)  11.  17.) 

Sp.  gr.  of  solution  sat.  at  18°  =  1.003  and 
contains  0.27%  LiF.  (Mylius,  B.  1897,  30. 
1718.) 

Sol.  in  800  pts.  H2O,  and  the  presence  of 
NH4F  and  NH3  decreases  solubility  to  1  : 
3500.  (Carnot,  Bull.  Soc.  1889,  (3)  1.  250.) 

Two  crystalline  forms  are  very  si.  sol.  in 
HC1;  easily  sol.  in  HNO3.  (Poulenc,  Bull. 
Soc.  1894,  (3)  11.  17.) 

Two  crystalline  forms  are  insol.  in  95% 
alcohol.  (Poulenc.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Difficultly  sol.  in  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Lithium  hydrogen  fluoride,  LiHF2. 

Difficultly  sol.  in  H2O,  but  more  easily  than 
LiF.  (Berzelius.) 

Lithium  silicon  fluoride. 
-See  Fluosilicate,  lithium. 

Lithium  stannic  fluoride. 
See  Fluostannate,  lithiuin. 

Lithium  tantalum  fluoride. 
See  Fluotantalate,  lithium. 

Lithium  uranyl  fluoride,  UO2F2,  4LiF. 

(Ditte.) 

Lithium  zirconium  fluoride. 
See  Fluozirconate,  lithium. 


Lithium  hydride,  LiH. 

Not    deliquescent.      Decomp. 
(Guntz,  C.  R.  1896,  123.  997.) 


by    H20. 


Lithium  hydrosulphide,  LiSH  (?). 

Deliquescent.  Sol.  in  H2O  and  alcohol. 
(Berzelius,  Pogg.  6.  439.) 

Lithium  hydroxide,  LiOH. 

Not  so  deliquescent  as  NaOH,  and  aj 
ently  not  more  sol.  in  hot  than  cold 
(Gmelin,  Glib.  62.  399.) 

Not  deliquescent.  (Arfvedson,  A.  ch.  10. 
82.) 

The  solubility  of  LiOH  in  H2O  can  be  ex- 
pressed by  y  =  6.6750+0.00346t+0.0003t2, 
where  y  =  the  percentage  of  Li2O  in  a  satur- 
ated solution.  (Dittmar,  Jour.  Soc.  Chem. 
Ind.  7.  730.) 

Solubility  of  LiOH  in  H2O  at  t°. 


t° 

G.  per  100  g.  Solution 

G.  LiOH  per 
100  g.  H2O 

Li20                   LiOH 

0 

6.67 

10.64 

12.7 

10 

6.74 

10.80 

12.7 

20 

6.86 

10.99 

12.8 

25 

6.95 

11.14 

12.9 

30 

7.05 

11.27 

12.9 

40 

7.29 

11.68 

13.0 

50 

7.56 

12.12 

13.3 

60 

7.96 

12.76 

13.8 

•  80 

8.87 

14.21 

15.3 

100 

10.02 

16.05 

17.5 

(Seidell's  Solubilities,  1st  Ed.  174.) 

A  sat.  aq.  solution  contains  7.09%  LiOH. 
(Schreinemakers,  C.  C.  1905,  II.  1486.) 

Sp.  gr.  of  LiOH+Aq  at  18°  containing: 
1.25         2.5  5        7.5%  LiOH. 

1.0132     1.0276     1.0547     1.0804 
(Kohlrausch,  W.  Ann.  1879.  1.) 

Solubility  in  Li3SbS4+Aq  at  30°. 


% 

LiOH 

% 
Li3SbS4 

Solid  Phase 

11.4 

0 

LiOH,  H20 

9.1 

8.3 

" 

2.3 

29.9 

u 

2  1 

48.3 

K 

2.1 

1.4 

52.1 
51.8 

LiOH,  H2O+Li3SbS4, 
Li3SbS4,  10H2O 

10H20 

0 

51.3 

(C 

(Donk,  Chem.  Weekbl.  1908,  5.  529,  629,  767.) 

SI.  sol.  in  alcohol;  insol.  in  alcohol-ether. 
(Mayer.) 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1904,  37..3601.) 


LITHIUM  SILICIDE 


459 


Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Cryst.  also  with  H2O,  and  M>H2O.  (Gottig, 
B.  20.  2912.) 

Lithium  imide,  Li2NH. 

Decomp.  at  high  temp.  Insol.  in  toluene, 
benzene,  ether  and  ethyl  acetate.  Decomp. 
CIIC13.  (Ruff,  B.  1911,  44.  506.) 

Lithium  iodide,  Lil. 
Deliquescent. 

Solubility  in  100  pts.  H2O  at: 
0°   19°  40°  59°   75°  80°   99°   120° 
151  164  179  200  263  435  476  588  pts.  Lil. 

Sp.  gr.  of  Lil+Aq  at  19.5°  containing: 
5          10        15        20        25         30%  Lil, 
1.038    1.079    1.124    1.172    1.224    1.280 

35        40        45        50        55         60%  Lil. 
1.344    1.414    1.489    1.575    1.670    1.777 
(Kremers,  Pogg.  104.  133;  111.  60:  Ger- 
lach,  Z.  anal.  8.  295.) 

Sp.  gr.  of  Lil+Aq  at  18°  containing: 
5  10  15  20  25%  Lil. 

1.0361     1.0756     1.1180     1.1643      1.2138 
(Kohlrausch,  W.  Ann.  1879.  1.) 

Temp,  of  maximum         g.-mol.  Lil  dissolved 

density  of  Lil+Aq.  in  1000  g.  H2O. 

2.516°  0.1795 

0.039°  0.4666 

(de  Coppet,  C.  R.  1900,  131.  178.) 

Very  sol.  in  liquid  NH3.  (Franklin,  Am. 
Ch.  J.  1898,  20.  828.) 

100  g.  methyl  alcohol  dissolve  343.4  g.  Lil 
at  25°. 

100  g.  ethyl  alcohol  dissolve  250.8  g.  Lil 
at  25°. 

100  g.  propyl  alcohol  dissolve  47.52  g.  Lil 
at  25°. 

100  g.  isoamvl  alcohol  dissolve  112.50  g. 
Lil  at  25°. 

In  the  case  of  propyl  alcohol  the  solid 
phase  at  25°  is  Lil,  4C3H8O.  (Turner  and 
Bissett,  Chem.  Soc.  1913,  103.  1909.) 

Solubility  in  organic  solvents  at  t°. 

C=pts.  by  wt.  of  Lil  in  100  ccm.  of  the 
sat.  solution. 

L=no.  of  liters  which  at  the  saturation 
temp,  hold  in  solution  1  mol.  Lil. 


Solvent 

'     t 

C 

L 

Furfurol 

Nitromethane 
tt 

25° 
25° 
0° 

45.86 
2.519 
1.219 

0.292 
5.32 
10.98 

(Walden,  Z.  phys.  Ch.  1906,  66.  718.) 

Solubility  in  glycol  at  15.3°  =  28%.     (de 
Coninck,  Belg.  Acad.  Bull.  1906,  359.) 

Sol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1369.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3789.) 

Difficultly  sol.  in  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899,  II. 
1014;  Naumann,  B.  1904,  37.  4328.) 

+H2O.    Mpt.   below  200°.    (Bogorodsky, 

.  C.  1897,  II.  175.) 

+2H2O.     Mpt.  86-88°.     (Bogorodsky.) 

+3H2O.    Mpt.  75°.    (Bogorodsky.) 

Sol.  in  absolute  alcohol  without  decomp. 
(Thirsoff,  Chem.  Soc.  1894,  66.  (2)  234.) 

The  composition  of  the  hydrates  formed  by 
Lil  at  different  dilutions  is  calculated  from 
determinations  of  the  lowering  of  the  fr.-pt. 
produced  by  Lil  and  of  the  conductivity  and 
sp.  gr.  of  Lil+Aq.  (Jones,  Am.  Ch.  J.  1905, 
34.  301.) 

Lithium  mercuric  iodide,  2LiI,  HgI2+6H2O. 

Very  deliquescent.  Decomp.  by  H2O. 
Very  sol.  without  decomp.  in  alcohols,  glycer- 
ine, acetone,  fuming  formic  acid,  acetic  acid, 
ethyl  acetate,  ethyl  oxalate,  etc.  Less  sol. 
in  nitrobenzene.  Insol.  in  benzene  and 
methyl  iodide.  (Duboin,  C.  R.  1905,  141. 
1017.) 

+8H2O.  Decomp.  by  H2O.  Very  sol.  in 
alcohols,  glycerine,  acetone^  fuming  formic 
acid,  acetic  acid,  ethyl  acetate,  etc.  without 
decomp.  SI.  sol.  in  nitrobenzene.  Insol.  in 
benzene  and  methyl  iodide.  (Duboin,  1.  c.) 

+9H2O.  Hydroscopic.  Sol.  in  alcohol 
and  acetone  without  decomp.  (Dobroserdoff, 
C.  C.  1901, 1.  664.) 

Lithium  nitride,  Li3N. 

Sol.  in  H2O  with  decomp.  (Ouvrard,  C.  R. 
114.  120.) 

Very  hydroscopic.  (Dafert,  M.  1910,  31. 
987.) 

Lithium  oxide,  Li2O. 

Slowly  sol.  in  H2O  to  form  LiOH. 
See  Lithium  hydroxide. 

Lithium  peroxide,  Li2O2. 

(de  Forcrand,  C.  R.  1900,  130.  1467.) 

Lithium  hydrogen  peroxide,   Li2O2,  H2O2  + 

3H2O. 

Sol.  in  H2O.  Insol.  in  alcohol,  (de  For- 
crand, C.  R.  1900,  130.  1466.) 

Lithium  selenide,  Li2Se. 

Sol.  in  H2O.    (Fabre,  C.  R.  103.  269.) 
+9H2O.    Sol.  inH2O.    (Fabre.) 

Lithium  silicide,  Li6Si2. 

Decomp.  by  H2O  and  by  dil.  acids.  De- 
comp. by  aqueous  solutions  of  alkalies  with 
evolution  of  H2.  (Moissan,  C.  R.  1902,  134. 
1083.) 


460 


LITHIUM  SULPHIDE 


Lithium  ?w(wosulphide,  Li2S. 

More  sol.  in  H2O  or  alcohol  than  LiOH. 

Luteochromium  bromide,  Cr(NH3)6Br3. 

Less  sol.  in  H2O  than  the  chloride.     (Jor- 
gensen,  J.  pr.  (2)  30.  1.) 

bromoplatinate,    [Cr(NH3)6]2(PtBr6)3 

4H2O. 

SI.  sol.  in  H2O.    Insol.  in  alcohol.    (Jorgen- 
sen.) 

chloride,  Cr(NH3)6Cl3+H2O. 

Efflorescent,  and  very  sol.  in  H2O.    (Jorgen- 


chloroplatinate. 

(a)  [Cr(NH3)6]2(PtCl6)3+6H2O.  Nearly 
completely  insol.  in  H2O.  (Jorgensen.) 

(6)  Cr(NH3)6Cl(PtCl6)+2^H2O.  Decomp. 
by  H2O  into  above;  insol.  in  alcohol.  (Jor- 
gensen.) 

(c)  [Cr(NH3)6i2Cl4(PtCl6)+2H20.  De- 
comp. by  H2O  into  (a).  (Jorgensen.) 

mercuric  chloride,  Cr(NH3)6Cl3,  HgCl2. 

Decomp.  by  H2O;  si.  sol.  in  dil.  HCl+Aq; 
insol.  in  alcohol. 

Cr(NH3)6Cl3,  3HgCl2+2H2O.  Decomp. 
by  dil.  HCl+Aq  into  above  salt.  (Jorgen- 
sen.) 

—  chromicyanide,  Cr(NH3)6Cr(CN)6. 
Precipitate. 

cobalticyanide,  Cr(NH3)6Co(CN)6. 

Nearly  insol.  in  H2O  or  in  cone.  HCl+Aq. 
(Jorgensen.) 

ferrocyanide,  Cr(NH3)6Fe(CN)6. 

Very  si.  sol.  in  cold  H2O  or  dil.  acids. 
(Jorgensen.) 

iodide,  Cr(NH3)6I3. 

SI.  sol.  in  H2O.     (Jorgensen,  1.  c.) 

iodosulphate,  Cr(NH3)6So4I. 

Sol.  in  H2O;  nearly  insol.  in  dil.  NH4OH  + 
Aq  or  alcohol.  (Jorgensen.) 

— -  nitrate,  Cr(NH3)6(NO3)3. 

Sol.  in  35-40  pts.  H2O.  Insol.  in  cold  dil. 
HNO3+Aq  or  alcohol.  Can  be  crystallised 
out  of  H2O  containing  a  little  HNO3.  (Jor- 
gensen, J.  pr.  (2)  30.  1.) 


— —  nitrate  chloroplatinate, 

Cr(NH3)6(NO3)PtCl6+H2O. 
Insol.  in  H2O.     Sol.  in  dil.  H2SO4+Aq. 
(Jorgensen.) 

nitratosulphate,  Cr(NH3)6(NO3)SO4. 

Sol.  in  H2O;  insol.  in  alcohol.    (Jorgensen.) 


Luteochromium  oxalate,  [Cr(NH3)6]2(C2O4)3  + 

4H2O. 
Nearly  insol.  in  cold  H2O.    (Jorgensen.) 

or^ophosphate,  Cr(NH3)6PO4+4H2O. 

SI.  sol.  in  H2O;  easily  sol.  in  dil.  acids. 
(Jorgensen.) 


sodium  pyrophosphate, 

Cr(NH3)6(NaP207)  + 


Nearly  insol.  in  cold  H2O;  wholly  insol.  in 
dil.  NH4OH+Aq.  (Jorgensen.) 

sulphate,  [Cr(NH3)6]2(SO4)3+5H2O. 

Quite  sol.  in  H2O;  insol.  in  alcohol.  (Jor- 
gensen.) 

sulphate  chloroplatinate, 

[Cr(NH3)6(SO4)]2PtCl6. 
Nearly  insol.  in  H2O.    (Jorgensen.) 

Luteocobalt  examine  chromium  sulpho- 
cyanide. 

See  Diamine  chromium  luteocobalt  sulpho- 
cyanide. 

Luteocobaltic  bromide,  Co(NH3)6Br3. 

Sol.  in  H20.  Precipitated  from  saturated 
H2O  solution  by  dil.  HBr+Aq.  (Jorgensen. 
J.  pr.  (2)  35.  417.) 


bromopermanganate, 

Co(NH3)6Br2(MnO4). 
Easily  sol.  in  H2O.    (Klobb,  A.  ch.  (6)  12. 


5.) 


bromoplatinate,  Co(NH3)6Br3,  PtBr4+ 
H2O. 

SI.  sol.  in  H2O;  can  be  recrystallised  from 
hot  H2O  containing  HBr.  (Jorgensen.) 

-  bromosulphate,  Co(NH3)6Br(SO4). 
Nearly  insol.  in  H2O.    Very  si.  sol.  in  dil. 

NH4OH+Aq.    (Jorgensen.) 

-  carbonate,  [Co(NH3)6]2(CO3)3+7H2O. 
Efflorescent;  easily  sol.  in  H2O. 
[Co(NH3)6]2(C03)3,    H2C03+5H20.      Less 

sol.  in  H2O  than  the  neutral  salt.     (Gibbs 
and  Genth.) 

—  chloride,  Co(NH3)6Cl3. 

Sol.  in  17.09  pts.  H2O  at  1(X50;  16.81  pts'. 
at  11.4°;  16.48  pts.  at  12°;  and  more  easily  in 
hot  H2O.  (F.  Rose.) 

100  pts.  H2O  dissolve  4.26  pts.  at  0°,  and 
12.74  pts.  at  46.6°.  (Kurnakoff,  J.  russ.  Soc. 
24.  629.) 

Not  appreciably  sol.  in  cone.  HCl+Aq. 
(Jorgensen.) 

Insol.  in  alcohol  or  solutions  of  the  alkali 
ihlorides.  (Gibbs  and  Genth.) 

Insol.  in  NH4OH+Aq. 


LUTEOCOBALTIC  CHROMATE 


461 


Aqueous  solution  is  pptd.  by  alcohol,  min- 
eral acids,  or  alkali  chlorides. 

Luteocobaltic  mercuric  chloride,  Co(NH3)6Cl3, 


Sol.  in  hot  H2O.    (Krok,  1870.) 

By  recrystallizing  from  hot  H20  containing 
HC1  is  converted  into  — 

Co(NH3)6Cl3,  3HgCl2+H2O.  Very  si.  sol. 
in  cold  H2O.  (Jorgensen.) 

Co(NH3)6Cl3,  2HgCl2  +  ^H2O.  Sol.  in  hot 
H2O,  from  which  it  crystallizes  on  cooling. 
Insol.  in  cold  cone.  HCl+Aq,  and  is  pptd. 
from  H2O  solution  by  HC1  or  alcohol.  (Car- 
stanjen.) 

Does  not  exist.    (Jorgensen.) 

+3H2O.  More  easily  sol.  in  cold  H2O  and 
other  solvents  than  the  preceding  comp. 
(Carstanjen,  Berlin,  1861.) 

Does  not  exist.    (Jorgensen.) 

-  stannous  chloride,  2Co(NH3)6Cl3, 
3SnCl2  +  10H2O. 

+8H2O. 

-  chloraurate,  Co(NH3)6Cl3,  AuCl3. 
Very  si.  sol.  in  cold,  more  easily  in  hot  H2O 

containing  HC1.    (Gibbs  and  Genth,  Sill.  Am. 
J.  (2)  23.  330.) 

-  chloriodate,  [Co(NH3)6Cl2]2I4O11+H2O. 

-  chloriridite,  Co(NH3)6,  IrCl6. 

Insol.   in  boiling  H2O   or  dil.   HCl+Aq. 

(Gibbs.) 

-  chloriridate,  2Co(NH3)6Cl3,  3IrCl4. 
Insol.  in  H2O.    (Gibbs.) 

-  chlorochromate,   Co(NH3)6CrO4Cl+ 
3H2O. 

Sol.  in  H2O.  (Klobb,  Bull.  Soc.  1901,  (3) 
26.  1027.) 

-  chlorofluoride,  Co(NH3)6Cl2F. 
(Bohm,  Z.  anorg.  1905,  43.  339.) 

—  chloropalladite,  2Co(NH3)6Cl3,  3PdCl2. 

Easily  sol.  in  dil.  HCl+Aq.  (Gibbs,  Sill. 
Am.  J.  (2)  37.  58.) 

-  chloroperchlorate,  Co(NH3)6Cl(ClO4)2. 
(Millosevich,  Gazz.    ch.   it.   1901,  31.  (2) 

285.) 

-  chloropermanganate, 

Co(NH3)6Cl2(MnO4). 

Can  be  recrystallized  from  H2O.  (Klobb, 
C.  R.  103.  384.) 

-  chloropermanganate  ammonium  chlor- 
ide, Co(NH3)6Cl2(MnO4),  NH4C1. 

Easily  sol.  in  H2O.    (Klobb.) 


Luteocobaltic  chloropermanganate  potassium 

chloride,  Co(NH3)6Cl2(MnO4),  KC1. 
Very  easily  sol.  in  H2O,  with  decomp.  into 
constituents;  sol.  in  KCl+Aq.    (Klobb.) 

chloropermanganate   sodium  chloride, 

Co(NH3)6Cl2(MnO4),  NaCl. 

Very  sol.  in  H20.    (Klobb.) 

chloroplatinate,  2Co(NH3)6Cl3,  3PtCl4  + 

6H2O. 

Can  be  recrystallized  from  much  hot  H2O. 
(Gibbs  and  Genth.) 

+21H2O.    (Gibbs  and  Genth.) 

Co(NH3)6Cl3,  PtCl4+^H2O.  Very  si.  sol. 
in  cold,  decomp.  by  hot  H2O  into — 

2Cp(NH3)6Cl3,  PtCl4+2H2O.  By  recrys- 
tallizing from  hot  H2O  containing  HC1  this 
salt  is  converted  into  the  above  salt.  (Jor- 
gensen.) 

chlororhodite. 

Nearly  insol.  in  boiling  H2O  or  dil.  acids. 
Sol.  in  cone.  HCl+Aq.  (Gibbs,  Sill.  Am.  J. 
(2)  37.  57.) 

chlororuthenate,  2Co(NH3)6Cl3,  3RuCl4. 

Sol.  in  dil.  acids.    (Gibbs.) 

chloroselenate,  Co(NH8)6ClSeO4+3H2O. 

Decomp.  by  H2O.  (Klobb,  Bull.  Soc. 
1901,  (3)  25.  1029.) 

chlorosulphate,  Co(NH3)6Cl(SO4). 

Sol.  in  H2O. 

+3H2O.  Only  si.  sol.  in  cold  H2O.  (Klobb, 
Bull.  Soc.  1901,  (3)  26.  1025.) 

ammonium  chlorosulphate, 

[Co(NH3)6]4Cl2(S04)5,     3(NH4)2S04+     . 
6H2O. 

Decomp.  by  H2O.  (Klobb,  Bull.  Soc. 
1901,  (3)  26.  1027.) 

chlorosulphate  chloroplatinate, 

2Co(NH3)6Cl(SO4),  PtCl4. 
Very  si.  sol.  in  cold  pure  H2O.  .Can  be  re- 
crystallized    out    of    H2O    containing    HC1. 

(Krok.) 

chlorosulphate  mercuric  chloride, 

Co(NH3)6Cl(S04),  HgCl2. 
Scarcely  sol.  in  pure  H2O,  but  can  be  crys- 
tallized from  warm  acidified  H2O.    (Krok.) 

chlorosulphite,    Co(NH3)6(SO8)Cl+ 

3H2O. 

Sol.  in  H2O.  (Vortmann  and  Magdeburg, 
B.  22.  2637.) 

chromate,  [Co(NH3)6]2(CrO4)3+5H2O. 


Ppt.    Sol.  in  hot  H2O. 
[Co(NH3)6]2(Cr20)3+5H20. 
sol.  in  hot  H2O. 


Moderately 


462 


LUTEOCOBALTIC  CHROMICYANIDE 


Luteoccbaltic  chromicyanide. 

Co(NH3)6Cr(CN)6. 
Ppt.     (Braun.) 

—  cobalticyanide,  Co(NH3)6Co(CN)6. 
Ppt. 

dithionate,  basic, 

4[Co(NH3)6(S206)(OH)],  Co2(S206)20. 
Sol.  in  H2O  and  dil.  alcohol. 

—  ferricyanide,  Co(NH3)6Fe(CN)6  + 
3^H20. 

Insol.  in  H2O.    (Braun.) 

— - —  fluoride,  Co(NH3)6F3. 

SI.  sol.  in  cold  H2O.  Nearly  insol.  in  acids. 
(Bohm,  Z.  anorg.  1905,  43.  340.) 

hydrogen  fluoride,  Co(NH3)6H3F6. 

SI.  sol.  hi  H2O.  Decomp.  by  hot  H2O. 
(Miolati  and  Rossi,  Real.  Ac.  Line.  1896, 
(5)  5.  II,  185.) 

hydrogen  boron  fluoride, 

Co(NH3)6F3,  3BF3,  HF. 
Cryst.  from  H2O  acidified  with  HF.    Mio- 
lati and  Rossi.) 

molybdenyl  fluoride, 

Co(NH3)6F3,  2  MoO2F2. 
Cryst.  from  H2O  containing  HF.    (Miolati 
and  Rossi.) 


silicon  fluoride, 

Co(NH3)6F3,    2SiF4. 
Rossi.) 


(Miolati    and 


titanium  hydrogen  fluoride, 

2Co(NH3)6F3,    3TiF4,    2HF. 
and  Rossi.) 


(Miolati 


tungstyl  fluoride, 

Co(NH3)6F3,    2WO2F2.      (Miolati    and 
Rossi.  ) 

uranyl  fluoride. 

Co(NH3)6F3,  UO2F2. 

Can  be  cryst.  from  H2O  containing  HF. 
(Miolati  and  Rossi.) 

vanadyl  fluoride, 

2Co(NH3)6F3,  5V02F,  7HF. 
Ppt.    (Miolati  and  Rossi.) 

fluoride  nitrate, 

Co(NH3)6F(N03)2. 
{Bohm,  Z.  anorg.  1905,  43.  336.) 

- — hydroxide,  Co(NH3)6(OH)3. 
Known  only  in  aqueous  solution. 


Luteocobaltic  mercuric  hydroxychloride, 

CoN6H14(HgCl)3(HgOH)Cl3. 
Ppt.      Easily    decomp.      (Vortmann    and 
Morgulis,  B.  22.  2644.) 
CoN6H14(HgOH)4Cl3.    Ppt.     (V.  and  M.) 
CoN6Hi6(HgOH)2Cl3.    Ppt.     (V.  and  M.) 

iodide,  Co(NH3)6I3. 

Insol.  in  cold,  but  moderately  sol.  in  hot 
H20. 

According  to  Jorgensen,  contains  HNO3  and 
has  the  formula  Co2(NH3)12I4(NO3)2. 

iodosulphate,  Co(NH3)6I(SO4). 

Can  be  recrystallized  from  hot  H2O.  SI. 
sol.  in  warm/  nearly  insol.  in  cold  H2O. 
(Krok,  B.  4.  711.) 

mercuriodide,  Co2Ni2H33(HgI)3I6. 

Ppt.    (Vortmann  and  Borsbach.) 
CoN6H16(HgI)2I3.    Ppt.    (V.  and  B.) 

mercuriodide,  basic, 

CoN6H16(HgOH)2I2(OH). 
Insol.  in  H2O.     SI.  sol.  in  H2O.     (Vort- 
mann and  Borsbach,  B.  23.  2804.) 

nitrate,  Co(NH3)6(NO3)3. 

Sol.  in  H2O.  Can  be  recrystallised  from 
boiling  H20.  Sol.  in  about  60  pts.  H2O. 
Insol.  in  cone.  HNO3+Aq.  (Jorgensen,  J. 
pr.  (2),  35.  417.) 

Almost  insol.  in  acids.  (Rogoiski,  A.  ch. 
(3),  41.  454.) 

Insol.  in  NH4OH,  HC1,  and  HNO3+Aq; 
decomp.  by  H2SO4+Aq.  (Gibbs  and  Genth.) 

Co(NH3)6(NO3)3,  HNO3.  Decomp.  by 
H2O  or  dil.  alcohol.  (Jorgensen,  J.  pr.  (2),  44. 
63.) 


nitrate  chloroplatinate, 


Co(NH3)6(NO3)Ch,   PtCl4+H2O. 
Not  decomp.  by  H2O.     (Jorgensen.) 

•  nitratosulphate,   Co(NH3)6(NO3)(SO4). 

Sol.  in  H2O.    (Jorgensen.) 

nitrite  cobaltic  nitrite, 

Co2(NH3)12(NO2)6,  Co2(NO2)6  = 

Co(NH,),(NOOeCo. 
Nearly  insol.  in  H2O.    (Jorgensen.) 
Much  less  sol.  in  H2O  than  the  correspond- 
ing roseo  salt.    (Gibbs.) 

•  diamine  cobaltic  nitrite, 

Co(NH3)6[Co(NH3)2(N02)4]3. 

Ppt.     (Gibbs.) 

=  Co(NH3)6](N02)2(NH3)2Co(N02)2]3. 
Nearly  insol.  in  cold,  si.  sol.  in  boiling  H2O. 
(Jorgensen,  Z.  anorg.  6.  179.). 

-  oxalate,  [Co(NH3)6]2(C2O4)3+4H20. 
Insol.  in  hot  or  cold  H2O.     Easily  sol.  in 
H2C2O4+Aq. 


LUTEOCOBALTIC  SULPHATE  BROMAURATE 


463 


Luteocobaltic  oxalate  chloraurate, 

2Co(NH3)6(C2O4)Cl,  AuCl3+4H2O. 
Easily  sol.  in  hot  H2O.    (Gibbs.) 

— -  perchlorate,  Co(NH3)6(ClO4)3. 

(Millosevich,  Gazz.  ch.   it.   1901,  31,   (2) 

285.) 

permanganate,  [Co(NH3)6]2(MnO4)3. 

Nearly  insol.  in  H2O.  100  pts.  H2O  at  0° 
dissolve  only  0.072  pt.  salt.  Moderately 
sol.  in  hot  H2O.  (Klobb,  A.  ch,  (6)  12.  5.) 

— — •  persulphate  sulphate, 

[Co(NH3)6]2S208(S04)2. 

Much  less  sol.  in  H20  than  the  sulphate. 

Sol.  in  641  pts.  H2O  at  18.8°  and  in  632 
pts.  at  20°.  Not  easily  sol.  even  in  boiling 
H2O.  (Jorgensen,  Z.  anorg.  1898,  17.  459.) 


or^ophosphate,     Co(NH3)6(PO4)  + 


4H2O. 

SI.  sol.  in  cold  H2O.    Easily  sol.  in  dil.  acids. 
(Jorgensen.) 

[Co(NH3)6]3(P04)(P04H)3+5KH20     (?). 
Ppt.    (Braun.) 

[Co(NH3)6]2(PO4H)3+4H2O.    Ppt.    Easily 
sol.  in  very  dil.  HCl+Aq.     (Jorgensen.) 

raetaphosphate. 

Ppt. 


p?/rophosphate,    [Co(NH3)6]2P4O13+ 

6H2O. 

(Gibbs,   Am.   Acad.   Proc.   11.   29);   or 
Co2(NH3)i2P4O13(ONa)2   (Vortmann,   B,   11. 
2181);    or   Co(NH3)6(P2O7Na)+ll^H2O. 
(Jorgensen,  J.  pr.  (2)  35.  438.) 

Very  nearly  insol.  in  H2O.     With  H2O  at 
80°  it  is  decomp.  into — 

[Co(NH3)6]4(P2O  )3+20H2O.     Less   easily 
sol.  than  the  preceding  salt. 

—  p*/rophosphate,  acid,  Co(NH3)6(P2O7H). 
Wholly  insol.  in  H2O.     Somewhat  sol.  in 

dil.  HC2H3O2+Aq.    Easily  sol.  in  HCl+Aq 
(Jorgensen.) 

sodium  ps/rophosphate, 

Co(NH3)6(P2O7Na)  +11^H2O. 
Ppt.      Not    wholly    insol.    in    cold    H2O. 
Decomp.  by  hot  H2O.    Less  sol.  in  NH4OH  + 
Aq  than  in  H2O.    (Jorgensen.) 

[Co(NH3)6]4(P2O7)3,     2Co(NH3)6(NaP2O7) 
+39  H20.  As  above.    (Jorgensen.) 

—  selenate,  [Co(NH6)]2(SeO4)3+5H2O. 
Very   sol.   in   H2O.      (Klobb,    Bull.   Soc. 

1901,  (3)  26.  1028.) 

hydrogen  selenate, 

[Co(NH3)6]H(SeO4)2+2^H2O. 
Not  decomp.  by  H2O.    .(Klobb.) 


Luteocobaltic  ammonium  selenate, 

[Co(NH3)6]2(Se04)3,    (NH4)2Se04+ 

4H2O. 

Very  sol.  in  H2O. 

[Co(NH6]2(SeO4)3,    (NH4)2SeO4+8H2O. 
Very  sol.  in  H2O.    (Klobb.) 

—    sulphocyanide,    Co(NH3)6(SCN)3. 

Decomp.  by  hot  H2O.    (Miolati,  Z.  anorg. 
1900,  23.  241.) 

mercuric  sulphocyanide, 

Co(NH3)6(SCN)3,  2Hg(SCN)2. 
Decomp.  by  H2O. 
Cryst.  from  dil.  NH4SCN+Aq.    (Miolati.) 

platinum  sulphocyanide, 

[Pt(SCN)4]3[Co(NH3)6(SCN3)]2. 
Decomp.  by  hot  H2O.    (Miolati.) 


silver  sulphocyanide, 


Co(NH3)6(SCN)3,  2AgSCN. 
Decomp.  by  hot  H2O.    (Miolati.) 

—  sulphate,  [Co(NH3)6]2(SO4)3+5H2O. 
SI.  sol.  in  cold,  more  easily  in  hot  H2O. 
+6H2O.  (Krok,B.4.711.) 


hydrogen  sulphate, 

.       Co(NH3)6H(S04)2. 

Decomp.   by  alcohol  to  sulphate, 
gensen,  Z.  anorg.  1898,  17.  458.) 


(Jor- 


4[(Co6NH3)2(SO4)3],  5H2SO4+10H2O. 
Very  sol.  in  H2O  with  decomp.  into  the  normal 
sulphate. 

When  pulverized  it  seems  to  dissociate 
slowly  in  contact  with  abs.  alcohol.  (Klobb, 
Bull,  Soc.  1901,  (3)  25.  1025.) 

ammonium  sulphate, 

[Co6(NH3)6]2(S04)3,  (NH4)2S04+8H20. 
Sol.  in  H20  with  decomp.     (Klobb.) 

cerium  sulphate,  [Co(NH3)6]2(SO4)3, 

Ce2(S04)3+l^H20. 

Very  si.  sol.  in  cold,  and  practically  insol. 
in  boiling  H2O.  Sol.  in  acids.  (Gibbs,  Am. 
Ch.  J.  15.  560.) 

[Co(NH3)6]2(S04)3,  3Ce(S04)2+H20.  As 
above.  (Wing,  Sill.  Am.  J.  (2)  49.  363.) 

— —  lanthanum  sulphate,  [Co(NH3)6]2(SO4)j, 

La,(S04),+H,0. 
SI.  sol.  in  H2O.    (Wing.) 

thallic      sulphate,      [Co(NH3)6]2(SO4)3, 

T12O(SO4)2+5H2O. 
Decomp.  by  cold  H2O.    (Gibbs.) 

sulphate  bromaurate, 

Co(NH3)6(S04)(AuBr4). 
Very  si.  sol.  in  H2O  with  apparent  decomp. 
Insol.  in  alcohol.     (Jorgensen.) 


464 


LUTEOCOBALTIC  SULPHATE  CHLORAURATE 


Luteocobaltic  sulphate  chloraurate. 

Co(NH3)6(SO4)AuCl4. 
SI.  sol.  in  H2O.    (Jorgensen.) 

cobaltic    sulphite,    [Co(NH3)6]2(SO3)3, 

Co2(SO3)3+H2O  =  dichrocobaltic        sul- 
phite,  [Co(NH3)3]2(SO3)3+2H2O,  which 
see. 

[Co(NH3)6]2(S03)3,  2Co,(SO,),+15H,0  = 
diamine  cobaltic  sulphite,  [Co(NH3)2]2(SO3)2 
+5H2O,  which  see. 

Luteorhodium  bromide,  Rh(NH3)6Br3. 

Less  sol.  in  H2O  than  the  chloride.  (Jor- 
gensen, J.  pr.  (2)  44.  51.) 

chloride,  Rh(NH3)6Cl3. 

Sol.  in  7  to  8  pts.  H2O  at  8°.    (J.) 
+H2O.     Extremely  efflorescent.     (J.) 

rhodium  chloride,  Rh(NH3)6Cl3,  RhCl3. 

Sol.  in  H2O.  (Jorgensen,  Z.  anorg.  5. 
174.) 

—  chloroplatinate,  2Rh(NH3)6Cl3,  3PtCl4+ 

6H20. 

Insol.inH2O.    Sol.in  warmHCl+Aq.    (J,) 
Rh(NH*)gCl»,    PtCl4+^H2O.      Decomp. 

by  H20  into  chloride  and  above  salt.    ( J.) 

nitrate,  Rh(NH3)6(NO3)3. 

Sol.  in  48  to  49  pts.  H2O  at  ord.  temp. 
HNO3+Aq  diluted  with  5  vols.  H2O  ppts. 
the  salt  completely  from  aqueous  solution. 
(Jorgensen,  J.  pr.  (2)  44.  51.) 

Rh(NH3)6(NO3)3,  HNO,.  Decomp.  by 
H2O  or  dil.  alcohol.  (Jorgensen,  J.  pr.  (2), 
44.  63.) 

or^ophosphate,    Rh(NH3)6P04+4H2O. 

SI.  sol.  in  cold  H2O.    (J.) 

sodium  p?/rophosphate, 

[Rh(NH3)6]2(P207)3Na2+23H20. 
Nearly  wholly  insol.  in  H2O.    Wholly  insol. 
inNH4OH+Aq.    (J.) 

sulphate,  [Rh(NH3)6]2(SO4)3+5H2O. 

Sol.  in  43  pts.  H2O  at  20°.    (J.) 

Magnesium,  Mg. 

Does  not  decomp.  H2O  at  ord.  temp.j  but 
decomp.  slowly  at  100°.  H2O  containing 
acids  dissolves  Mg  easily.  Sol.  in  cold  dil. 
HC2H3O2+Aq.  Difficultly  sol.  in  cold 
H2SO4+Aq.  (Bunsen.)  Cold  nitrosulphuric 
acid  does  not  attack.  (Bunsen.)  Cold 
NH4OH+Aq,  KOH+Aq,  or  NaOH+Aq  do 
not  attack.  (Maak,  Phippson.)  Sol.  in  NH4C1 
or  (NH4)2CO3-f  Aq.  (Wohler.) 


Very  rapidly  sol.  in  K2S2O8+Aq  and 
(NH4)2S2O8+Aq  with  violent  evolution  of 
gas.  (Levi,  Gazz.  ch.  it.  1908,  38.  (1),  583.) 

Attacked  by  aqueous  solution  of  KCL 
NH4C1,  NaCl,  LiCl,  CuCl2,  CdCl2,  CoCl2, 
PbCl2,  HgCl2,  FeCl3,  CrCl,,  PtCl4,  AuCl3, 
CuSO4,  ZnSO4,  FeSO4  and  MnSO4. 

SI.  attacked  by  hot  30%  CaCl2+Aq,  not 
by  30%  MgCl2+Aq,  BaCl2+Aq  and  SrCl2  + 
Aq.  (Tommasi,  Bull.  Soc.  1899,  (3),  21.  886.) 

Not  attacked  by  NH4F+Aq,  very  slowly 
by  solutions  of  BaCl2,  CaCl2,  KC1,  K3Fe(CN)6, 
NaNO8,  Na2S2O3  and  Na2HPO4.  Solutions 
of  NaC2H3O2,  Na2B4O,,  alum  and  chrome 
alum  attack  vigorously.  Solutions  of 
(NH4)2C03,  NH4C1,  (NH4)2C204,  (NH4)2S 
and  Na2CO3  attack  even  more  vigorously. 
(Mouraour,  C.  R.  1900,  130.  140.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 

Insol.  in  liquid  HF.  (Franklin,  Z.  anorg. 
1905,  46.  2.) 

Somewhat  sol.  in  liquid  NH3,  if  a  clean 
metallic  surface  is  in  contact  with  the  pure 
solvent.  (Kraus,  J.  Am.  Chem.  Soc,  1907, 
29.  1561.) 

^ccm.  oleic  acid  dissolves  0.0104  g. 
Mg  in  6  days.  (Gates,  J.  phys.  Chem.  1911, 
15.  143.) 

Magnesium  arsenide,  Mg3As2. 

Decomp.  on  air.  (Parkinson,  Chem.  Soc. 
5.  127.) 

Magnesium  azoimide,  Mg(N3)2. 

Decomp.  by  hot  H2O.  (Curtius,  J.  pr. 
1898,  (2)  58.  292.) 

Magnesium  boride,  Mg9B2. 
Sol.  in  HCl+Aq.    (Winkler,  B.  23.  774.) 

Magnesium  bromide,  MgBr2. 

Deliquescent.  Very  sol.  in  H2O  with  evolu- 
tion of  heat. 

Sat.  MgBr2-f-Aq  contains  at: 
—18°      +1-7°     48°       62°       97° 

52          58      60.9     62.5     65.8%  MgBr2. 
(fitard,  A.  ch.  1894,   (7),  2.  541.) 

See  also  MgBr2+6H2O. 

Sp.  gr.  of  MgBr2+Aq  at  19.5°  containing: 
5  10         15         20         25  %  MgBr2, 

1.043    1.087    1.137   1.191    1.247 

30         35       40  45         50  %  MgBr2. 

1.31      1.377    1.451    1.535   1.625 
(Kremers,    Pogg.    108.    118,    calculated    by 
Gerlach,  Z.  anal.  8.  285.) 

MgBr2+Aq  is  si.  decomp.  by  evaporation. 


MAGNESIUM  BROMIDE 


465 


Solubility  of  MgBr2  in  alcohols. 

MgBr2  forms  with  methyl  alcohol  a  com- 
plex, MgBr2,  6CH3OH. 

Solubility  of  MgBr2,  6CH3OH  in  CH8OH  at  t° 

Solubility  of  MgBr2,  6(iso)C4H9OH  in 
C4H9OH  at  t°. 

t° 

%  by  weight 
of  MgBr2, 
6isoC4H»OH 

t° 

VKSff* 

6isoC4H9OH 

0 
10 
20 
30 
40 
50 

55.8 
60.5 
65.2 
69.8 
74.3 
78.5 

60 
65 
71 
75 

77 
80  mpt. 

82.4 
84.2 
88.0   ' 
92.0 
94.6 
100 

t° 

%  by  weight 
of  MgBr2, 
6CH3OH 

t° 

%  by  weight 
of  MgBr2, 
6CH3OH 

0 
20 
40 
60 
80 
100 
110 
120 

42.6 
44.6 
46.7 
48.9 
51.4 
55.5 
58.0 
60.7 

130 
140 
150 
160 
170 
180 
185 
190  mpt. 

63.6 
66.8 
70.2 
74.0 

78.5 
84.5 
88.0 
100 

(Menschutkin.) 

MgBr2  forms  with  isoamylalcohol  a  com- 
plex, MgBr2,  6(iso)C5HnOH. 

Solubility  of   MgBr2,    6(iso)C6HnOH   in 
C6HnOH  at  t°. 

(Menschutkin,  Z.  anorg.  1907,  62.  11.) 

MgBr2  forms  with  ethyl  alcohol  a  complex, 
MgBr2,  6C2H5OH. 

Solubility  of  MgBr2,  6C2H6OH  in  C2H6OH 
at  t°. 

t° 

%  by  weight 
of  MgBr2, 
GisoCsHnHO 

t° 

%  by  weight 
of  MgBr2, 
GisoCsHnOH 

0 
10 
20 
30 
35 

70.2 
75.6 
80.2 
84.5 
86.7 

38 
40 
42 
44 
46  mpt 

88.7 

90.0 
92.0 
94.2 
100 

t° 

%  by  weight 
of  MgBr2, 
6C2H5OH 

t° 

%  by  weight 
of  MgBr2, 
6C2H6OH 

(Menschutkin.) 
Solubility  in  ether  at  t°. 

t° 

%  MgBr2 

%  MgBr2,  2C4HioO 

0 
10 
20 
30 
40 
50 
60 
70 
75 

17.2 

24.9 
32.7 
40.3 
47.8 
55.1 
62.2 
68.8 
71.4 

80 
85 
90 
95 
100 
103 
106 
108.  5  mpt. 

73.8 
76.2 
78.7 
82.3 
86.7 
90.0 
94.4 
100 

—  8 
0 
+  10 
14 
16 
18 
20 
22  mpt. 

0.6 

0.8 
1.27 
1.64 
1.93 
2.3 
2.7 
3.22 

1.08 
1.44 
2.3 
2.95 
3.48 
4.14 
4.86 
5.80 

(Menschutkin.) 

MgBr2  forms  with  propyl  alcohol  a  com- 
plex, MgBr2,  6C3H7OH. 

Solubility  of  MgBr2,  6C8H7OH  in  C3H7OH 

att°. 


Solubility  of  MgBr2,  2C4Hi0O  in  ether  at  t°. 
'Lower  solution"=the  melted  MgBr2, 
2C4Hi0O  which  does  not  mix  with  the  ether 
above. 


t°  ' 

%  by  weight 
of  MgBr2, 
6C3H7OH 

t° 

%  by  weight 
of  MgBr2, 
6C3H7OH 

0 
10 
20 
30 
40 

77.9 
81.5 
85.1 
89.5 
92.0 

43 
46 
48 
50 
52  mpt. 

93.0 
94.3 
95.8 

97.8 
100 

(Menschutkin.) 

MgBr2  forms  with  isobutylalcohol  a  com- 
plex, MgBr2,  6(iso)C4H9OH. 


t° 

Composition  of 
lower  solution 

Composition  of  the 
upper  layer 

%  MgBr2 

lc»' 

%  MgBr, 

%  MgBr2, 
2C4H100 

—10 

42.0 

75.7 

1.8 

3.2 

0 

41.0 

73.9 

2.3 

4.1 

+10 

40.1 

72.2 

2.8 

5.0 

20 

39.3 

70.8 

3.3 

5.9 

30 

38.7 

69.8 

3.8 

6.8 

40 

38.2 

68.8 

4.3 

7.7 

50 

37.8 

68.0 

4.7 

8.5 

60 

37.6 

67.7 

5.1 

9.2 

70 

37.6 

67.7 

5.4 

9.7 

80 

37.8 

68.0 

5.6 

10.0 

90 

38'.  1 

68.6 

5.7 

10.2 

(Menschutkin.) 

466 


MAGNESIUM  BROMIDE 


Solubility  of  MgBr2  in  formic  acid. 
MgBr2  forms  with  formic  acid  a  complex, 
MgBr2,  6HCOOH. 

Solubility  of  MgBr2,  6HCOOH  in  HCOOH 
att°. 


Solubility  of  MgBr2  in  acetone. 
MgBr2    forms    with    acetone    a    complex. 
MgBr2,  3CH3COCH3. 

Solubility  of  MgBr2,  3CH3COCH3  in 
CH3COCH3  at  t°. 


t° 

%  by  wt.  MgBr2,  6HCOOH 

t° 

%  by  wt.  MgBr2, 
3CH3COCH3 

0 
20 
40 
60 
70 
80 
86 
88  mpt. 

49.8 
57.5 
65.1 
73.1 
78.1 
86.0 
95.0 
100 

0 
30 
60 
70 

72 
73 
74 
75 
76 
80 
84 
88 
92  mpt. 

0.2 
0.8 
1.45 
2.0 
3.7 
5.5 
14.0 
50.0 
71.6 
83.3 
89.8 
95.2 
100 

(Menschutkin,  Z.  anorg.  1907,  64.  90.) 

Solubility  of  MgBr2  in  acetic  acid. 
MgBr2  forms  with  acetic  acid  a  complex. 
MO-HT...  ftnTT-nnnw 

Solubility  of  MgBr2,  6CH3COOH  in 
CH3COOH  at  t°. 

Solubility  of  MgBr2  in  acetamide. 
MgBr2  forms  with  acetanide  a  complex, 
MgBr2,  6CH3CONH2. 

Solubility  of  MgBr2,  6CH3CONH2  in 
CH3CONH2  at  t°. 

t° 

%  by  wt.  MgBr2, 
GCHsCOOH 

17 
30 
50 
60 
70 
80 
85 
90 
100 
105 
110 
112  mpt. 

0.3 
1.5 
4.5 
7.9 
16.2 
38.5 
49.5 
57.7 
71.8 
80.0 
89.5 
100.0 

t 

%£H%^' 

50.5 
70 
90 
110 
130 
150 
'-'     160 
165 
169  mpt. 

56.0 
57.8 
60.5 
65.0 
71.5 
80.0 
85.5 
90.0 
100.0 

(Menschutkin.) 

Solubility  of  MgBr2  in  acetic  anhydride. 
MgBr2  forms  with  acetic  anhydride  a  com- 
plex, MgBr2,  6(CH3CO)2O. 

Solubility  of  MgBr2,  6(CH3CO)2O  in 
(CH3CO)2O  at  t°. 


(Menschutkin,  Z.  anorg.  1909,  61.  106.) 

Solubility  of  MgBr2  in  acetanilide. 
MgBr2  forms  with  acetanilide  a  complex, 
MgBr2,  6CH3CONHC6H5. 

Solubility  of  MgBr2,  6CH3CONHC6H5  in 
CH3CONHC6H5  at  t°. 


t° 

%  by  wt.  MgBr2, 
6(CH3CO)20 

t 

%  by  wt.  MgBr2, 
6CH3CONHC6H5 

0 

26.4 

107.5 

9.0 

30 

30.0 

140 

19.3 

60 

37.7 

170 

29.6 

90 

44.5 

185 

39.0 

120 

57.8 

195 

49.0 

130 

69.8 

200 

59.5 

135 

85.0 

205 

73.2 

136-137  mpt. 

100     . 

209  mpt. 

100.0 

(Menschutkin,  Z.  anorg.  1909,  61.  112.) 

(Menschutkin,  Z.  anorg.  1909,  61.  109.) 

MAGNESIUM  BROMIDE 


467 


Solubility  of  MgBr2  in  aniline. 

MgBr2  forms  with  aniline  three  complexes: 
MgBr2,  6C6H5NH2;  MgBr2,  4C6H5NH2: 
MgBr2,  2C6H5NH2. 

Solubility  of  these  complexes  in  aniline. 


Solubility  of  MgBr2  in  methylal. 
MgBr2  forms  with  methylal  a  complex, 
MgBr2,  2CH2(OCH3)2. 

Solubility  of  MgBr2,  2CH2(OCH3)2  in 
CH2(OCH3)2  at  t°. 


Solubility  of  MgBr2,  6C6H6NH2  in  C6H5NH2. 

t° 

%  by  wt.  MgBr2, 
2CH2(OCH3)2 

t° 

%  by  weight  of  MgBr2, 
6C6H5NH2 

» 

20 
40 
60 
80 
100 
106 
106 
108 
110 
112  mpt. 

0.3 
0.45 
0.6 
0.75 
0.9 
1.1 
86.2 
90.8 
95.4 
100 

10 
30 
50 
70 
90 
100 
103.5 

3.2 
3.9 
5.1 
7.5 

12.8 
18.5 
27.5 

Solubility  of  MgBr2,  4CeH5NH2  in  C6H5NH2. 

(Menschutkin,  Z.  anorg.  1907,  53.  32.) 

Solubility  of  MgBr2  in  dimethylcarbinol. 
MgBr2    forms    with    dimethylcarbinol    a 
complex,  MgBr2,  4(CH3)2CHOH. 

Solubility  of  MgBr2,  4(CH3)2CHOH  in 
(CH3)2CHOH  at  t°. 

t° 

%  by  weight  of  MgBr2, 
4C«H5NH2 

103 
120 
140 
160 
180 
200 
220 
230 
237 

24.0 
24.3 
24.9 
26.0 
28.3 
33.5 
45.0 
55.0 
76.3 

t° 

%  by  weight 
of  MgBr2, 
4(CH3)2CHOH 

%  by  weight 
t°                   of  MgBr2, 
4(CH3)2CHOH 

0 
20 
40 
60 
80 
100 

40.0 

42.2 
45.0 
48.5 
53.3 
59.0 

110                     62.5 
120                     67.3 
130                     74.0 
136                      83.6 
138                      90.00 
139  mpt.           100 

Solubility  of  MgBr2,  2C6H5NH2  in  C6H5  NH2 

t 

%  by  weight  of  MgBrj, 
2C6H5NH2 

237 
250 
260 
270 

76.3 
77.3 

78.1 
79.0 

(  M  enschutkin  .  ) 

Solubility  of  MgBr2  in  trimethylcarbinol. 
MerBr*    forms    with    trimethvlcarbinol    a 

(Menschutkin,  Z.  anorg.  1907,  62.  159.)         complex,  MgBr2,  4(CH3)3COH. 


Solubility  of  MgBr2  in  benzaldehyde. 
MgBr2  forms  with  benzaldehyde  a  com- 
plex, MgBr2,  3C6H5CHO. 

Solubility  of  MgBr2,  3C6H5CHO  in 
C6H5CHO  at  t°. 


Solubility  of  MgBr2,  4(CH3)3COH  in 
(CH3)3COH  at  t°. 


t 

%  by  wt.  MgBtt, 
3C6H5CHO 

t 

%  by  wt.  MgBr2, 
SCeHsCHO 

0 

0.7 

140 

17.8 

30 

1.3 

145 

37.5 

60 

1.9 

146 

65.0 

80 

2.5 

148 

84.5 

100 

3.4 

153 

93.2 

120 

6.0 

159  mpt. 

100 

130 

9.5 

(Menschutkin,  Z.  anorg.  1907,  63.  26.) 


t° 

%  by  weight 
of  MgBr,, 
4(CH3)3COH 

t° 

%  by  weight 
of  MgBr2, 
4(CH3)3COH 

24.4 
25 
35 
45 
55 
60 

0.06 
1.0 

9.5 
19.1 
32.2 
40.5 

65 
70 
75 

77.5 
79 
80  mpt. 

50.5 
62.5 
77.0 
85.0 
91.5 
100 

Menschutkin.) 

Solubility  of  MgBr2  in  phenylhydrazine. 
MgBr2  forms  with  CeHsNHNH^  a  complex. 
MgBr2,  6C6H6NHNH2. 

468 


MAGNESIUM  MANGANOUS  BEOMIDE 


Solubility  of  MgBr2,  6C6H5NHNH2  in 
C6H5NHNH2  at  t°. 

MgBr2,    6NH2COOC2H5    decomposes    at 
90.5-91°  forming  MgBr2,  4NH2COOC2H5. 

Solubility  of  MgBr2,  4NH2COOC2H5  in 
NH2COOC2H6  at  t°. 

t° 

%  by  wt.  of  MgBr2, 
6C6H5NHNH2 

20 
40 
60 
80 
99 
100 
140 
180 
200 

3.0 
7.0 
16.4 
33.0 
54.8 
54.8      • 
60.8 
68.4 
73.4 

t° 

%  by  wt.  MgBr2, 
4NH2COOC2H5 

91 
100 
110 
115 
120 
123  mpt. 

69.4 
73.8 
80.0 
84.1 
90.0 
100.0 

(Menschutkin,  Z.  anorg.  1907,  52.  162.) 

Solubility  of  MgBr2  in  urea. 
MgBr2  forms  with  urea  a  complex,  MgBr2, 
6CO(NH2)2. 

Solubility  of  MgBr2,  6CO(NH2)2  in  urea  at  t°' 

(Menschutkin.) 
+6H2O. 

Solubility  of  MgBr2+6H2O  in  H2O  at  t°. 

t° 

%  by  weight 
of  MgBr2  + 
6H2O 

t° 

%  by  weight 
of  MgBr2  + 
6H20 

t° 

^NlS?1* 

0 
20 
40 
60 
80 
100 

76.0 

78.1 
80.2 
82.3 
84.4 
86.6 

120 
140 
150 
160 
164  mpt. 

89.0 
92.0 
94.9 
98.0 
100 

108.5 
115 
120 
125 
127 
130 

24.2 
29.8 
35.0 
41.6 
45.5 
60.0 

(Menschutkin,  Z.  anorg.  1907,  52.  153.) 

(Menschutkin,  Z.  anorg.  1909,  61.  116.) 

MgBr2,   6CO(NH2)2  decomposes   at   130° 
giving  MgBr2,  4CO(NH2)2. 

Solubility  of  MgBr2,  4CO(NH2)2  in  urea  at  t°. 


t° 

-      %  by  wt.  MgBr2, 

4CO(NH2)2 

130 
145 
160 
165 
170 
171 

58.0 
60.7 
67.2 
71.4 
83.7 
96.0 

(Menschutkin,  Z.  anorg.  1909,  61.  116.) 

Solubility  of  MgBr2  in  urethane. 
MgBr2  forms  with  urethane  a  complex, 
MgBr2,  6NH2COOC2H6. 

Solubility  of  MgBr2,  6NH2COOC2H5  in 
NH2COOC2H5  at  t°. 


35 
50 
70 
80 
85 
90 
*91.5 


by  wt.  MgBr2, 
2COOC2H5 


43.3 
45.6 
51.3 
56.2 
59.8 
66.5 
75.5 


*  Mpt.  of  MgBr2,  6NH2COOC2H5. 
(Menschutkin,  Z.  anorg.  1909,  61. 


Sp.  gr.  of  solution  sat.  at  18°  =  1.655,  and 
contains  50.8%  MgBr2.  (Mylius  and  Funk, 
B.  1897,  30.  1718.) 

SI.  sol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

Sol.  in  alcohol.  Sol.  in  acetone.  (Nau- 
mann,  B.  1904,  37.  4328;  Eidmann,  C.  C. 
1899,  II.  1014.) 

Difficultly  sol.  in  methyl  acetate.  (Nau- 
mann,  B.  1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

+  10H2O.  Sol.  in  H2O.  (Panfiloff,  Chem. 
Soc.  26.  234.) 

Magnesium  manganous  bromide,  MgBr2, 

2MnBr2  +  12H2O. 

Deliquescent.  (Saunders,  Am.  Ch.  J.  14. 
150.) 

Magnesium  mercuric  bromide,  MgBr2,  HgBr2 


MgBr2,  2HgBr2.    Not  deliquescent. 

Magnesium    molybdenyl    bromide,    MgBr2, 
MoOBr3+7H2O.    ' 

(Weinland  and  Knoll,  Z.  anorg.  1905,  44. 
112.) 

Magnesium     potassium     bromide,     MgBr2, 

2KBr+6H2O. 

Easily  sol.  in  H2O,  from  which  KBr  crys- 
tallises at  75  to  87°.  Alcohol  dissolves  out 
MgBr2.  (Lowig,  Repert.  29.  261.) 


MAGNESIUM  CHLORIDE 


469 


Formula    is    MgBr2,    KBr+6H20.      De- 

Sp. gr.  of  MgCl2-t-Aq  at  15°. 

liquescent.    (Lerch,  J.  pr.  (2)  28.  338.) 

Magnesium  stannic  bromide. 

-£? 
§ 

o 

o 

See  Bromostannate,  magnesium. 

M 

Sp.  gr. 

j 

Sp.  gr. 

1 

Sp.  gr. 

Magnesium  chloride,  MgCl2. 

&5 

£5 

55 

Deliquescent.      Very    sol.    in    H2O    with 

1 

1.0084 

13 

1.1130 

2-5 

1.2274 

evolution  of  heat.    The  solution  decomposes 

2 

1.0169 

14 

1  .  1220 

26 

1.2378 

on  evaporation  losing  HC1,  when  less  than  6 

3 

1.0253 

15 

1.1311 

27 

1.2482 

mols.   H2O   are  present   to    1   mol.    MgCl2. 

4 

1.0338 

16 

1  .  1404 

28 

1.2586 

(Casaseca,  C.  R.  37.  350.) 

5 

1.0422 

17 

1.1498 

29 

1.2690 

Anhydrous.    Sol.  in  1.857  pts.  H2O  at  15°. 

6 

.0510 

18 

.1592 

30 

1.2794 

(Gerlach.) 

7 

.0597 

19 

.1686 

31 

1.2903 

Sol.  in  1  pt.  cold  H20.     (Fourcroy.) 
Sat.    MgCl2+Aq   at    12.5°   contains   64.8%    MgCl2. 

8 
9 

.0684 
.0772 

20 
21 

.1780 
.1879 

32 
33 

1.3012 
1.3121 

(Hassenfratz.) 
100  pts.  H2O  at  15.5°  dissolve  200  pts.  MgCU.    (Ure's 
Diet.) 

10 
11 

.0859 
.0949 

22 
23 

.1977 
.2076 

34 
35 

1.3230 
1.3340 

12 

1040 

24 

.2175 

100  pts.  H2O  dissolve  52.2  pts.  MgCl2  at  0° 

and  sp.  gr.  of  sat.  solution  =  1.36  19  at  15°. 

rr\  i  u    rr    „„„!    o    001   \ 

1000  mols.  H26  dissolve  108  mols.  MgCl2 
at  25°C.  (Lbwenherz,  Z.  phys.  Ch.  1894,  13. 
479.) 


Sp.  gr.  of  MgCl2+Aq  at  18°. 


100  mols.  MgCl2+Aq  contain  at  t°: 
t°            67.5     68.5     68.7     79.5     79.95 
Mol.MgCl2  11.58   11.92   11.71    12.28   12.39 

t°             116.67  152.6     181-2        186 
Mol.  MgCl2       16.2       18.24    23.8   24.1-24.4 
(Vant  Hoff  and  Meyerhoffer,  B.  A.  B.  1897, 

73.) 

Solubility  of  MgCl2  in  H2O  at  t°. 

|          Sp.  gr. 

1 
£S 

Sp.  gr. 

o 

g          Sp.  gr. 

5      1.0416 
10      1.0859 

20 
30 

1.1764 
1.2779 

34      1.3210 

(Kohlrausch,  W.  Ann.  1879.  1.) 

Sp.  gr.  of  MgCl2+Aq  at  0°.    S=pts.  salt  in 
100  pts.  of  solution;  Si  =  mols.  salt  in  100 
mols.  solution. 

t° 

MgCl2 

Solid  phase 

—10 
—20 
—30 
—33.6 
—20 

11.4 
16. 
19.4 
20.6 
26.7 
30.5 
31.6 

34.3 

34.6 
34.9 
35.3 
35.6 
36.5 
37.9 
39.8 
42.2 
46.1 

49.1 

55.8 

56.1 

Ice 
K 

Ice+MgCl2,  12H20 

MgCl2,  12H2O 
tt 

MgCl2,  12H20  + 
MgCl2,  8H2O 
MgCl2,  8H20+MgCl2, 
6H2O 

MgCl2,  6H2O 
n 

MgCl2,  6H20+MgCl2, 
4H20 
MgCl2,  4H2O 
MgCl2,  4H20+MgCl2, 
2H20 
MgCl2,  2H20 

—16.4 

1ft    Q 

s 

Si 

Sp.  gr. 

—  3.4 

0 
10 
20 
22 
40 
60 
80 
100 
116.7 

152.6 
181.5 

186 

29.2056 
20.9293 
15.7989 
11.3249 
6.2008 

7. 
4. 
3. 
2. 
1. 

230 
762 
423 
355 
233 

1.2788 
1.1927 
1.1427 
1.1007 
1.0545 

(Charpy,  A.  ch.  (6)  29.  23.) 
Sp.  gr.  of  MgCl2+Aq  at  19.5°. 

Pts.  MgCl2 
in  100  pts.          Sp.  gr. 
H20 

Pts.  MgClz 
in  100  pts.          Sp.  gr. 
H20 

10.7          1.0826 
22.0          1.1592 

35.3          1.2388 
51.5          1.3235 

(Landolt-Bornstein,  Tab.  5th  Ed.  1912.  480.) 
See  also  MgCl2+6H2O. 

(Kremers, 

Pogg.  104.  155.) 

470 


MAGNESIUM  CHLORIDE 


Sp.  gr.  of  MgCl2+Aq  at  14°. 

Sp. 

gr.  ofMgC!2+Aq. 

go 

Sp.  gr. 

| 

Sp.  gr. 

1 

Sp.  gr. 

V*  MgCl2  g.  in  1000  g. 
of  solution 

Sp. 

gr.  16°/16° 

0 
0.4400 
0.8801 
1.7780 
3.4533 
7.4691 
14.7187 
29.6307 

.  1 
1 
1 
1 
1 
1 
1 
1 

.000000 
.000372 
.000741 
.001458 
.002888 
.006219 
.012235 
.024647 

0 
1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 

0.9993 
.0033 
.0073 
.0113 
.0154 
.0194 
.0234 
.0274 
.0314 
.0355 
.0395 
1.0435 
1.0476 
1.0517 
1.0558 
1.0599 
1.0641 

17 

18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 

1.0682 
1.0724 
1.0765 
1.0807 
1.0849 
1.0891 
1.0933 
1.0976 
1.1018 
1.1061 
1.1103 
1.1146 
1.1189 
1  .  1232 
1  .  1275 
1.1319 
1.1363 

34 
35 
36 
37 
38 
39 
40 
41 
42 
43 
44 
45 
46 
47 
48 

1.1407 
1.1451 
1.1495 
1.1540 
.1584 
.1628 
.1673 
.1718 
.1763 
.1809 
.1855 
1.1901 
1.1948 
1.1995 
1.2042 

(Dijken,  Z.  phys.  Ch.  1897,  24.  108.) 

Sp.  gr.  of  MgCl2  at  20.1°. 
p=per  cent  strength  of  solution;  d  =  ob- 
served duesity;  w  =  volume  cone,  in  grams 

per  cc.  (  Joo=w-) 

P 

d 

w 

28.83 
25.59 
20.31 
15.79 
10.185 
8.058 
5.919 
3.913 
'    3.903      * 
1.743 

1.2569 
1.2241 
1.1735 
1  .  1324 
1.0833 
1.0650 
1.0473 
1.0304 
1.0240 
1.0126 

0.36237 
0.31327 
0.23842 
0.17877 
0.11033 
0.08583 
0.06198 
0.04022 
0.03210 
0.01765 

(Oudemans,  Z.  anal.  7.  420.) 
Sp.  gr.  of  MgCl2+Aq  at  24°. 

I 

Sp.  gr. 

1 

Sp.  gr. 

1 

Sp.  gr. 

(Barnes,  J.  Phys.  Chem.  1898,  2.  546.) 
Sp.  gr.  of  MgCl2+Aq  at  t°. 

2 
4 
6 
8 
10 
12 
14 
16 
•  18 
20 
22 
24 
26 
28 

1.0069 
1.0138 
1.0207 
1.0276 
1.0345 
1.0415 
1.0485 
1.0556 
1.0627 
1.0698 
1.0770 
1.0842 
1.0915 
1.0988 

30 
32 
34 
36 
38 
40 
42 
44 
46 
48 
50 
52 
54 
56 

1.1062 
1.1137 
1.1212 
1.1288 
1  .  1364 
1  .  1441 
1.1519 
1.1598 
1.1677 
1.1756 
1  .  1836 
1.1918 
1.2000 
1.2083 

58 
60 
62 
64 
66 
68 
70 
72 
74 
76 
78 
80 

1.2167 
1.2252 
.2338 
.2425 
.2513 
.2602 
.2692 
.2783 
.2875 
.2968 
.3063 
.3159 

t° 

Concentration  of  MgCh+Aq 

Sp.  gr, 

23 
24 

1  pt.  MgCl2  in  8.1874  pts.  H2O 
1  pt.        "     "  102.1      "      " 

1.0906 
1.0065 

(Hittorf,  Z.  phys.  Ch.  1902,  39.  628.) 

Sp.  gr.  of  MgCl2  at  0°. 
G.  MgCl2  in  100  ccm.  of  solution  6.7158  9.9506 
Sp.  gr.                                            1.0591  1.0845 

G.  MgCl2  in  100  ccm.  of  sol.      13.8111  20.004 
Sp.  gr.                                          1.1106    1.1605 
(Bremer,  C.  C.  1902,  I.  293.) 

(Gerlach,  Z.  anal.  8.  283.     Calculated  from 
Schiff.) 

Sp.  gr.  of  MgCl2+Aq  at  25°. 


Concentration  of  MnCh+Aq. 

Sp.  gr. 

1-normal 
Vr-      " 

V«-    " 

Vr-      " 

1.1375 
1.0188 
1.0091 
1.0043 

(Wagner,  Z.  phys.  Ch.  1890,  6.  38.) 

Sp.  gr.  of  MgCl2+Aq  at  20°  containing  M 
g.  mols.  MgCl2  per  1. 

M         0.00493    0.007327      0.01      0.03104 
Sp.  gr.  1.000344  1.000524  1.000842  1.002756 

M         0.05108    0.07171        0.10          0.25 
Sp.  gr.  1.004224  1.006036  1.008505  1.020966 

M  0.50          0.75      0.9415 

Sp.  gr.  1.038496  1.056905  1.069617 

(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38.  699.) 


MAGNESIUM  MERCURIC  CHLORIDE 


471 


MgCl2+Aq  containing  10%  MgCl2  boils  at 
101.6°;  containing  20%  MgCl2  boils  at  106.2°; 
containing  30%  MgCl2  boils  at  115.6°.  (Ger- 
lach.) 

Sat.  MgCl2+Aq  forms  a  crust  at  122.5°, 
and  contains  52.9  pts.  MgCl2  to  100  pts.  H2O. 
(Gerlach,  Z.  anal.  26.  426.) 

B.-pt.  of  MgCl2+Aq.    P=pts.  MgCl2  to  100 
pts.  H20. 


B.-pt. 

p 

B.-pt. 

p 

B.-pt. 

P 

101° 

4.9 

111° 

34.6 

121° 

50.8 

102 

9.2 

112 

36.6 

122 

52.2 

103 

13.2 

113 

38.4 

123 

53.6 

104 

16.7 

114 

40.2 

124 

55.0 

105 

19.9 

115 

41.8 

125 

56.4 

106 

22.5 

116 

43.4 

126 

57.7 

107 

25.0 

117 

44.9 

127 

59.0 

108 

27.5 

118 

46.4 

128 

60.3 

109 

29.9 

119 

47.9 

129 

61.6 

110 

32.3 

120 

49.4 

130 

62.9 

Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.  257.) 

SI.  sol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1369.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

+2H2O.  Very  deliquescent.  (Ditte,  A. 
ch.  1881,  (5)  22.  560.) 

+4H2O.    (van't  Hoff  and  Meyerhoffer.) 

+6H2O.     Deliquescent.     Sol.   in  0.6  pt. 


(Gerlach,  Z.  anal.  26.  440.) 
B.-pt.  of  MgCl2+Aq  containing  %  MgCl2. 


%  MgCl2 

B.-pt. 

%  MgCl2 

B.-pt. 

4.6 

8.4 

101° 
102 

11.6 
14.3 

103° 
104 

(Skinner,  Chem.  Soc.  61.  341.) 

Sol.  in  KCl+Aq  at  50°.     (Uhlig,  C.  C. 
1913,  II.  749.) 

Sol.  in  7  pts.  alcohol  at  15°.     (Bergmann.) 
'     5     '  moderate  heat.     (.B) 

100  pts.  alcohol  of  given  sp.  gr.  dissolve  pts.  MgCl2: 


Sp.  gr. 

Pts.  MgCh 

Sp.gr. 

Pts.  MgCh 

0.900 

0.848 

21.25 
23.75 

0.834 
0.817 

36.25 
50.00 

cold,  and  0.273  pt.  hot  H2O.    (Casaseca,  I.  c.) 
Solubility  in  H2O  at  t°. 

t° 

1000  mols  H2O 
dissolve  mols 
MgCl2 

100  g.  H2O  dis- 
solve g.  MgCh 

3.5 
25.0 
50.0 

99.6 
104.5 
110.6 

52.65 
55.26* 
58.66 

(Biltz  and  Marcus,  Z.  anorg.  1911,  71.  169.) 

Solubility  in  KCl+NH4Cl+Aq  at  25°  has 
been  studied.    (Biltz  and  Marcus.  Z.  anorg. 
1911,  71.  178.) 
When  the  solid  phases  are  MgSO4+6H2O 
and  MgCl2+6H2O,  1000  mols.  H2O  dissolve 
104  mols.  MgCl2  and  14  mols.  MgSO4  at  25°. 
(Lowenherz,  Z.  phys.  Ch.  1894,  13.  480.) 

Solubility  of  MgCl2+6H2O  in  (NH4)MgCl8+ 
6H2O+Aq  at  t°. 

t° 

Per  1000  mols  H2O 

Mols  NH4C1 

Mols  MgCh 

3.5 
25.0 
50.0 

0.5 
0.5 
0.8 

99.5 
103.8 
111.2 

(Biltz  and  Marcus,  Z.  anorg.  1911,  71.  170.) 

(Kirwan.) 

MgCl2+6H2O  is  sol.  in  5  pts.  alcohol  of  0.90  sp.  gr. 
and  in  2  pts.  alcohol  of  0.817  sp.  gr. 

Sol.  in  0.1828  pt.  strong  alcohol  at  82.5°.      (Wenzel.) 

B.-pt.  of  an  alcoholic  solution  of  MgCl2. 


%  MgCl2 

B.-pt. 

5.56 
8.53 
9.62 
13.84 

78.  43°  +0.73° 
"      +1.34 
"      +1.77 
"      +3.54 

(Skinner,  Chem.  Soc.  61.  341.) 

Even  more  sol.  in  acetic  ether  than  CaCl2. 
(Cann,  C.  R.  102.  363.) 

Sol.  in  boiling  amyl  alcohol.  (Riggs,  Sill. 
Am.  J.  144.  103.) 

SI.  sol.  in  anhydrous  pyridine.  Sol.  in 
97%,  95%  and  93%  pyridine+Aq.  (Kahlen- 
berg,  J.  Am.  Chem.  Soc.  1908,  30.  1107.) 


Solubility  data  of  MgCl2+KCl+MgKCl, 
are  given  by  van't  Hoff  and  Meyerhoffer. 
(Z.  phys.  Ch.  1899,  30.  64.) 

+8H2O.  Pptd.  from  an  aqueous  solution 
which  contains  about  10  mols.  H2O  to  1  mol. 
MgCl2. 

+  12H2O.  Pptd.  from  an  aq  .  solution  which 
contains  1  mol.  MgCl2  in  about  12.06  mols. 
of  H2O.  (Bogorodsky,  C.  C.  1899,  1.  246.) 

Magnesium  manganous  chloride,  MgCl2) 
2MnCl2+12H2O. 

Deliquescent.  Very  sol.  in  H2O  and  al- 
cohol. (Saunders,  Am.  Ch.  J.  14.  148.) 

2MgCl2,MnCl2+12H2O.  Ppt.  Deliquesces 
in  the  air.  (Gossner,  C.  C.  1904,  1.  707.) 


Magnesium  mercuric  chloride,  MgCl2, 
+6H2O. 

Very  deliquescent.    More  sol.  than  the  fol- 
lowing salt.    (v.  Bonsdorff,  Pogg.  17.  133.) 

MgCl2,  3HgCl2+5H2O.    Sol.  in  H2O  with- 


472 


MAGNESIUM  PHOSPHORYL  CHLORIDE 


out   decomp.     Easily   sol.   in   alcohol,      (v. 
Bonsdorff.) 

Magnesium    phosphoryl    chloride.     MgCl2, 

POC18. 

Deliquescent.  Sol.  in  H2O  with  evolution 
of  heat  and  decomposition.  Very  si.  sol.  in 
warm  POC13.  (Casselmann,  A.  98.  223.) 

Magnesium  potassium  chloride.  MgCl2, 
2KC1+6H20. 

Deliquescent,  forming  a  solution  of  MgCl2, 
while  KC1  remains  undissolved.  100  pts.  H2O 
dissolve  64.5  pts.  at  18.75°.  20  pts.  salt  dis- 
solved in  80  pts.  H2O  lower  the  temp.  1.75°. 
(Bischof.)  Alcohol  dissolves  out  MgCl2.  De- 
comp. into  the  two  salts  by  solution  in 
H2O.  (Marcet.) 

A  sat.  solution  in  contact  with  solid  KC1 
and  KC1,  MgCl2,  H2O  at  50°  contains  79.5 
mol.  MgCl2  and  14.9  mol.  KC1  per  1000  mol. 
H2O.  A  sat.  solution  in  contact  with  solid 
MgCl2,  6H2O  and  KC1,  MgCl2,  H2O  at  50° 
contains  111.9  mol.  MgCl2  and  1.2  mol.  KC1 
per  1000  mol.  H2O.  (Uhlig,  Chem.  Soc.  1913, 
104.  (2)  775;  C.  B.  Miner.  1913,  417.) 

Min.  Carnallite. 

Magnesium  rubidium  chloride,  MgCl2,  RbCl 

+6H20. 

Not  decomp.  by  a  small  quantity  of  H20. 
(Feit  and  Kubierscky,  Ch.  Ztg.  16.  335.) 

Magnesium  sodium  chloride,  MgCl2,  NaCl+ 

2H20. 
Sol.  in  H2O.    (Poggiale.) 

Magnesium  thallic  chloride,  2T1C13,  MgCl2+ 

6H2O. 

Hydroscopic.  Can  be  cryst.  from  H2O. 
(Gewecke,  A.  1909,  366.  224.) 

Magnesium  stannic  chloride. 
See  Chlorostannate,  magnesium. 

Magnesium  vanadium  chloride,  MgCl2,  VC13 

+H20. 

Difficultly  sol.  in  H2O  and  alcohol.  (Stab- 
ler, B.  1904,  37.  4412.) 

Magnesium  zinc  chloride,  MgCl2,  ZnCl2+ 

6H2O. 

Deliquescent;  sol.  in  H2O.  (Warner,  C.  N. 
27.  271.) 

Magnesium  chloride  ammonia,  MgCl2,  4NH3. 
Easily  decomp.    (Clark,  A.  78.  369.) 

Magnesium  chloride  hydroxylamine,  MgCl2, 

2NH2OH+2H2O. 

100  g.  of  solution  in  H2O  contain  44.4% 
at  20°.  (Antonow,  J.  Russ.  Phys.  Chem. 
Soc.  1905,  37.  478.) 


Magnesium  fluoride,  MgF2. 

1  1.  H2O  dissolves  76  mg.  MgF2  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1904,  60.  356.) 

87  mg.  are  dissolved  in  1  1.  of  sat.  solution 
at  18°.  (Kohlrausch,  Z.  phys.  Ch.  1908,  64. 
168.) 

Scarcely  sol.  in  acids.  (Gay-Lussac  and 
Thenard.)  Insol.  in  excess  of  HF.  When 
precipitated,  is  sol.  in  aqueous  solution  of 
ammonium  and  magnesium  salts.  Sol.  in  dil. 
HNO3+Aq,  from  which  it  is  precipitated  by 
alcohol. 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Min.  Sellaile. 

Magnesium  potassium  fluoride,  MgF2,  KF. 

Decomp.  by  H2SO4.  (Duboin,  C.  R.  1895, 
120.  679.) 

MgF2,  2KF.  Decomp.  by  H2SO4.  (Du- 
boin.) 

Magnesium  sodium  fluoride,  MgF2,  NaF. 
Insol.  in  H20.    (Geuther,  J.  B.  1865.  173.) 

Magnesium  stannic  fluoride. 
See  Fluostannate,  magnesium. 

Magnesium  titanium  fluoride. 
See  Fluotitanate,  magnesium. 

Magnesium  zirconium  fluoride. 
See  Fluozirconate,  magnesium. 

Magnesium  hydrosulphide,  MgS2H2. 

Known  only  in  aqueous  solution,  which 
decomposes  on  warming.  Solution  contain- 
ing 16%  MgS2H2  has  sp.  gr.  1.118  at  12°. 
(Divers  and  Shimidzu,  Chem.  Soc.  46.  699.) 

Magnesium  hydroxide,  MgO2H2. 

MgO  is  sol.  in  55,368  pts.  EbO  at  ordinary  temp.,  and 
also  at  100°.  (Fresenius,  A.  59.  117.) 

MgO  is  sol.  in  5142  pts.  H2O  at  15.5°  (Fyfe) ;  in  5800 
pts.  at  15.8°  (Henry,  J.  Pharm.  13.  2) ;  in  7900  pts.  (Kir- 
wan) ;  in  16,000  pts.  (Dalton);  in  100,000-200,000  pts. 
cold  H2O  (Bineau);  in  36,000  pts.  boiling  HaO  (Fyfe, 
Ed.  Phil.  J.  5.  305.) 

Calculated  from  electrical  conductivity  of 
MgO2H2+Aq,  1  1.  H2O  dissolves  9  mg. 
MgO2H2  at  18°.  (Kohlrausch  and  Rose,  Z. 


phys.  Ch.  12.  241.) 
Calculated 


from  electrical  conductivity,  1 
1.  H2O  dissolves  00.076  g.  MgO2H2  at  18°. 
(Dupre*  and  Brutus,  Z.  angew.  Ch.  1903,  16. 
55.) 

Presence  of  CaO2H2  or  CaSO4  does  not  de- 
crease the  solubility.  (Henry.)  Presence  of 
the  salts  of  the  alkali  metals,  especially  am- 
monium salts,  increase  the  solubility.  Insol. 
in  cone.  Na2SO4,  NaNO3,  NaCl,  or  KNO3  + 
Aq.  (Karsten.)  Sol.  in  NH4OH+Aq,  but 
insol.  in  KOH+Aq.  (Odling.) 

Easily  sol.  in  acids.  Sol.  in  an  aqueous 
solution  of  sugar.  Boiling  alcohol  dissolves 
traces. 


MAGNESIUM  IODIDE 


473 


Solubility  of  MgO2H2  in  NH4Cl+Aq 
at  29°. 


ai 

ISI 


0.7 

0.466 

0.35 

I  0.23 

[0.17 


1121 


0.09835 

0.1108 

0.09835 

0.1108 

0.1108 


Normality  of 


MgOsH,    NH4C1 


0.156 
0.108 
0.089 
0 . 0638 
0.049 


0.388 
0.250 
0.172 
0.106 
0.0771 


G.  per  1. 


MgO*H8    NH4C1 


4.55 
3.15 
2.60 
1.86 
1.43 


20.86 

13.39 

9.21 

5.67 

4.13 


(Herz  and  Muhs,  Z.  anorg.  1909,  38.  140.) 
Solubility  of  MgO2H2  in  NH4NO3+Aq  at  29°. 


Cone  of 
NH4NOs 

+Aq 
(Nor- 
mal) 

Acid  re- 
quired 
for  liber- 
ated NH3 
in  25cc. 
(Normal) 

Normality  of 

G.  per  1. 

MgO2H2 

NH4NO3 

MgOjHj 

NH4N03 

0.35 
0.175 

0.1108 
0.1108 

0.0833 
0.0495 

0.1834 
0.076 

2.43 
1.45 

14.69 
6.09 

(Herz  and  Muhs.) 

^"Completely  insol.  in  16%  NaCl+Aq  in 
presence  of  0.8  g.  NaOH.  (Maigret,  Bull. 
Soc.  (3)  33.  631.) 

Solubility  of  MgO2H2  in  NaCl+NaOH+Aq. 


G.  NaCl  per  1. 

G.  MgO  per  1.  of  solution  with  added 

0.8  g.  NaOH  per  1. 

4.0  g.  NaOH  per  1. 

125 
140 
160 

0.07 
0.045 
None 

0.03 
None 

(Maigret.) 

Freshly  pptd.  Mg(OH)2  is  sol.  in  Th(NO3)4 
+Aq  forming  a  colloidal  solution.  (Halla, 
Z.  anorg.  1912,  79.  262.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II,  1014.) 

See  also  Magnesium  oxide. 

Min.  Brucite.  Sol.  in  cold  citric  acid+Aq. 
(Bolton,  C.  N.  37.  14.) 

2MgO,  3H20.    (Bender,  B.  3.  932.) 

Magnesium  iodide,  MgI2. 

Very  deliquescent. 

Solubility  in  H2O.   See  MgI2 +6,  and  8H2O. 

Sp.  gr.  of  MgI2+Aq  at  19.5°  containing: 
'5          10        15        20        25       30%MgI2, 
1.043   1.088  1.139   1.194  1.254  1.32 

35        40        45        50        55       60%  MgI2. 
1.395   1.474  1.568   1.668  1.78    [1.915 
(Kremers,  Pogg.  111.  62,  calculated  by 
Gerlach,  Z.  anal.  8.  285.) 

MgI2+Aq  decomp.  slightly  on  evaporation. 
Very  sol.  in  liquid  NH3.     (Franklin,  Am. 
Ch.  J.  1898,  20.  828.) 

Sol.  in  alcohol,  ether,  and  wood-spirit. 


Solubility  of  MgI2  in  alcohols. 
MgI2  forms  with  methyl  alcohol  a  complex, 
MgI2,  6CH3OH. 

Solubility  of  MgI2,  6CH3OH  in  CH3OH  at  t°. 


0 

20 
40 
60 
80 
100 


%  by  weight  of 
MgI2,  CH3OH 


49.6 
52.6 
55.3 
58.0 
60.6 
63.3 


120 
140 
160 
180 
200 


j  by  weight  of 
£gls,  6CH3OH 


66.2 
69.5 
73.2 
77.1 
81.5 


(Menschutkin,  Z.  anorg.  1907,  52.  15.) 

MgI2  forms  with  ethyl  alcohol  a  complex, 
MgI2,  6C2H5OH. 

Solubility  of  MgI2, 6C2H5OH  in  C2H5OH  at  t°. 


t° 

%  by  weight 
of  MgI2, 
6C2H5OH 

t° 

%  by  weight 
of  MgI2, 
6  C2H5OH 

0 
20 
40 
60 
80 
100 
110 

21.9 
33.2 
44.4 
55.3 
65.5 
74.7 
78.8 

120 
130 
135 
140 
143 
145 
146.5  mpt. 

82'.  7 
87.2 
90.0 
93.3 
96.0 
98.0 
100 

(Menschutkin.) 

MgI2  forms  with  dimethylcarbinol  a  com- 
plex, MgI2,  6(CH3)2CHOH. 

Solubility  of  MgI2,  6(CH3)2CHOH  in 
(CH3)2CHOH  at  t°. 


t° 

%  by  weight 
of  MgI2, 
6(CHS)2CHOH 

t° 

%  by  weight 
of  MgI2, 
6(CH3)2CHOH 

10 
30 
50 
70 
90 

57.1 
60.0 
63.3 
67.0 
71.2 

110 
120 
130 
136 
138  mpt. 

76.2 

79.4 
84.8 
91.7 
100 

(Menschutkin.) 
Solubility  of  MgI2  in  ether  at  t°. 


t° 

%  MgI2 

%  Mgls,  2C4HioO 

5.4 
11.8 
15.6 
18.1 
20.4 
22.2 

1.45 
2.43 
3.46 
5.4 
7.55 
11.28 

2.2 
3.7 
5.3 

8.3 
11.6 
17.3 

(Menschutkin,  Z.  anorg.  1906,  49.  41.) 


474 


MAGNESIUM  IODIDE 


t° 

%  MgI2 

%  MgI2,  2C4HioO 

Solubility  of  MgI2  in  acetone. 
MgI2  forms  with  acetone  a  complex,  MgI2l 
6CH3COCH3. 

Solubility  of  MgI2,  6CH3COCH3  in 
CH3COCH3  at  t°. 

in  lower  layer 

14.8 
17.6 
20 
28.4 
33 
35 

35.5 
35.5 
35.8 
35.5 
35.7 
35.3 

54.4 
54.4 
54.8 
54.4 
54.7 
54.1 

t° 

%  by  wt.  MgI2)  6CH3COCH3 

0 
30 
50 
60 
70 
80 
85 
90 
95 
100 
105 
106.  5  mpt. 

4.9 
6.7 
8.3 
10.2 
15.2 
28.6 
40.0 
59.2 
80.0 
92.5 
98.5 
100 

in  upper  layer 

18.6 

23.2 

24.4 
32.4 

13.57 
14.4 
14.6 
15.82 

20.8 
22.1 
22.4 
24.2 

in  solution  when  two  layers  mix 

37.3 
38.5 
38.5 
38.5 

38 

19.4 
22.45 
26.07 

29.8 
32.8 

29.3 
34.4 
39.9 
45.7 
50.3 

(Menschutkin,  Z.  anorg.  1907,  53.  30.) 

Solubility  of  MgI2  in  acetal. 
MgI2  forms  with  acetal  a  complex,  MgI2t 
2CH3CH(OC2H5)2. 

Solubility  of  MgI2,  2CH3CH(OC2H6)2  in 
CH3CH(OC2H5)2  at  t°. 

(Menschutkin.) 

Solubility  of  MgI2  in  acetic  acid. 
MgI2  forms  with  acetic  acid  a  complex, 
MgI2,  6CH3COOH. 

Solubility  of  MgI2,  6CH3COOH  in 
CH3COOH  at  t°. 

t° 

%  by  wt.  MgI2, 
2CH3CH(OC2H5)2 

20 
60 

77 
77 
79 
81 
83 
86  mpt. 

0.15 
0.45      .. 
0.6 
92.0 
93.7 
95.5 
97.3 
100 

t° 

%  by  wt. 

MgI2,  GCHsCOOH 

20 
40 
60 
70 
75 
80 
85 
95 
105 
115 
125 
135 
140 
142  mpt. 

0.6 
2.0 
5.0 
9.5 
13.0 
18.5 
27.1 
42.0 
54.5 
65.0 
73.8 
85.0 
94.0 
100.0 

(Menschutkin,  Z.  anorg.  1907,  53.  33.) 

Solubility  of  MgI2  in  acetamide. 
MgI2   forms  with   acetamide  a  complex, 
MgI2,  6CH3CONH2. 

Solubility  of  MgI2,  6CH3CONH2  in 
CH3CONH2  a_t  t°. 

t° 

%^c&12' 

49 
80 
110 
130 
150 
160 
170 
175 
177  mpt. 

56.5 
63.4 
70.5 
76.0 
82.1 
85.5 
90.8 
96.2 
100.0 

(Menschutkin,  Z. 

anorg.  1907,  54.  93.) 

(Menschutkin,  Z.  anorg.  1909,  61.  108.) 

MAGNESIUM  IODIDE 


475 


Solubility  of  MgI2  in  acetonitrile. 
MgI2  forms  with  acetonitrile  a  complex, 
MgI2,  6CH3CN. 

Solubility  of  MgI2,  6CH3CN  in  CH3CN 

att°. 


Solubility  of  MgI2  in  methyl  acetate. 
MgI2  forms  with  ethyl  acetate  a  complex, 
MgI2,  6CH3COOC2H5. 

Solubility  of  MgI2,   6CH3COOC2H5    in 
CH3COOC2H5  at  t°. 


t° 

%  by  wt.  MgI2,  6CH3CN 

t° 

%  by  wt.MgI2, 
6CH3COOC2H5 

0 
30 
50 
70 
80 
89 

37.2 
!           49.8 
58.2 
,   .    67.9 
76.5 
91.3 

0 
20 
40 
50 
55 
60 
65 
70 
75 
78  .  5  mpt. 

3.2 
4.8 
8.6 
13.7 
21.5 
38.0 
63.5 
90.5 
97.7 
100.0 

(Menschutkin,  Z.  anorg.  1909,  61.  110.) 

Solubility  of  MgI2  in  benzaldehyde. 
MgI2  forms  with  benzaldehyde  a  complex, 
MgI2,  6C6H5CHO. 

(  M  enschutkin  .  ) 

Solubility  of  MgI2,  6C6H6CHO  in  C6H6CHO 

att°. 


(Menschutkin,  Z.  anorg.  1907,  53.  28.) 

Solubility  of  MgI2  in  methyl  acetate. 
MgI2  forms  with  methyl  acetate  a  complex, 
MgI2,  6CH3COOCH3. 


Solubility  of  MgI2  in  ethyl  formate. 
MgI2  forms  with  ethyl  formate  a  complex, 
MgI2,  6HCOOC2H5. 


t° 

%  by  wt.  MgI2,  GCeHsCHO 

Solubility  of  MgI2,  6HCOOC2H5  in 
HCOOC2H5  at  t°. 

0 

3.2 

20 
40 

3.8 
5.3 

t° 

%  by  wt.  MgI2,  6HCOOC2H5 

60 

7.7 

o 

I  K     1 

80 
100 
110 

11.0 
18.5 
26.5 

10 
20 

on 

17.4 
20.5 

120 

40.0 

40 

Q1     C 

125 

53.0 

50 

44 

130 

74.5 

60 

fiS 

133 
136 

86.0 
94.2 

70.5  mpt. 

100 

139  mpt. 

100 

(Menschutkin.) 

Solubility  of  MgI2  in  isoamylacetate. 
MgI2  forms  with  isoamylacetate  a  complex, 
MgI2,  6CH3COO(iso)C5Hn. 

Solubility  of  MgI2,  6CH3COO(iso)C5Hu  in 
CH3COO(iso)C6Hu  at  t 


Solubility  ol  Mgi2,  6U±13(JUUCJ13  in 
CH3COOCH3  at  t°. 

t° 

%  by  wt.  MgL>, 
6CH3COO(iso)C5Hn 

t° 

GCHsCOOCHs' 

0 
20 
40 
45 
50 
55 
57.5 
60  mpt. 

7.7 
11.5 
20.9 
25.5 
33.2 
47.8 
63.0 
100.0 

0 
30 
60 
90 
100 
103 
103 
110 
120 
121  mpt. 

0.4 
0.55 
0.75 
0.9 

1.8 
2.4 
74.2 
81.7 
98.0 
100.0 

(Menschutkin.) 

Solubility  of  MgI2  in  isobutyl  acetate. 
MgI2  forms  with  isobutylacetate  a  com- 
plex, MgI2,  6CH3COOC4H9. 

(Menschutkin,  Z.  anorg.  1909,  61.  101.) 

476 


MAGNESIUM  MERCURIC  IODIDE 


Solubility  of  MgI2,  6CH3COO(iso)C4H9  in 
CH3COO(iso)C4H9. 

+8H2O.    Sp.  gr.  of  solution  of  MgI2+8H2O 
sat.  at  18°  containing  59.7%  MgI2  =  1.909. 
(Mylius,  B.  1897,  30.  1718.) 

Solubility  of  MgI2+8H2O  in  H2O  at  t°. 

t° 

%  by  wt.  MgI2, 
6CH3COO(iso)C4H9 

0 
20 
40 
50 
60 
70 
75 
80 
85 
87.5mpt. 

10.5 
13.6 
17.6 
20.4 
24.9 
33.7 
40.5 
52.0 
89.0 
100.0 

t° 

%  by  weight  of  MgI2  +8HzO 

•0 
20 
40 
43.5 

76.0 
81.0 

88.0 
90.8 

(Menschutkin.) 

+10H20.    Sol.  in  H20.    (Pdnfiloff,  C.  C. 
1894,  II.  610.) 

( M  enschutkin . ) 

Solubility  of  MgI2  in  propyl  acetate. 
MgI2  forms  with  propyl  acetate  a  complex, 
MgI2,  6CH3COOC3H7. 

Solubility  of  MgI2,  6CH3COOC3H7  in 
CH3COOC3H7  at  t°. 


t 

%  by  wt.  MgI2, 
6CH3COOC3H7 

0 

4.1 

20 

5.4 

30 

6.5 

35 

7.8 

40 

19.0 

45 

46.0 

50 

72.5 

55 

88.2 

60 

96.0 

65  mpt. 

100.0 

(Menschutkin.) 

Solubility  of  MgI2  in  urethane. 
MgI2  forms  with  urethane  a  complex,  MgI2, 
6NH2COOC2H6. 

Solubility  of  MgI2,  6NH2COOC2H5  in 
NH2COOC2H5  at  t°. 


t° 

%  by  wt.  MgI2, 
6NH2COOC2H5 

32 
50 
70 
80 

84 

87 

mpt. 

51.8 

59.4 
70.7 
78.8 
85.0 
100.0 

(Menschutkin.) 
+6H2O. 
Solubility  of  MgI2+6H2O  in  H2O  at  t°. 

t° 

%  by  weight  of            ,  0 
MgI2+6H20 

%  by  weight  of 
MgI2+6H20 

43° 
80° 
120° 

89.8             160° 
90.3             200° 
90.9             215° 

91.7 
93.4 
94.3 

(Menschutkin,  Z.  anorg.  1907,  52.  156.) 

Known  only  in  solution. 

+9H2O.  Very  deliquescent.  (Duboin, 
C.  R.  1906,  142.  1338.) 

Very  sol.  in  ethyl,  methyl,  propyl,  butyl, 
isobutyl,  amyl,  isopropyl*  and  allyl  alcohols, 
ethyl,  amyl,  propyl  and  isobutyl  acetates, 
ethyl  cyanide  and  acetone.  Sol.  in  benzyl 
alcohol.  Decomp.  by  glycerine.  SI.  sol.  in 
ethyl  benzoate,  amyl  benzoate,  nitrobenzene. 
Decomp.  by  ethyl  oxalate.  Insol.  in  toluene, 
benzene,  ethyl  iodide,  CHC13,  CC14,  ethylene 
bromide,  monochlor  and  monobrombenzene. 
(Duboin,  A.  ch.  1909,  (8)  16.  276.) 

MgI2,  2HgI2.  -Decomp.  by  H2O  into  HgI2 
and  above  compound,  which  remains  in  solu- 
tion. (Boullay.) 

+7H2O.  Sat.  solution  in  H2O  at  17.8°  has 
the  composition  MgI2,  1.29  HgI2,  11.06  H2O. 
(Duboin,  C.  R.  1906,  142.  1338.) 

Magnesium  potassium  iodide,  MgI2,  KI  + 

6H2O. 

Deliquescent.     (Lerch,  J.  pr.  (2)  28.  338.) 
Very  hygroscopic,    (de  Schulten,  Bull.  Soc. 

1900  (3)  23.  158.) 

Magnesium  iodide  ammonia,  MgI2,  6NH3. 

Practically  insol.  in  liquid  NH3.  (Franklin, 
J.  Am.  Chem.  Soc.  1913,  35.  1459.) 

Magnesium  nitride,  Mg3N2. 

Decomp.  by  moist  air  or  H2O.  Sol.  in  dil. 
or  cone.  HCl+Aq,  or  HNO3+Aq.  Sol.  in 
warm  H2SO4.  Insol.  in  alcohol,  ethyl  iodide, 
or  phosphorus  oxychloride.  (Briegleb  and 
Geuther,  A.  123.  236.) 

Decomp.  by  H2O.  (Smits,  R.  t.  c.  1894, 
12.  198.) 

Easily  decomp.  H2O  when  finely  powdered. 
(Rossel,  C.  R.  1895,  121.  942.) 

Magnesium  sw&oxide  (?). 

Decomp.  H2O.  Sol.  in  dil.  acids.  (Beetz, 
Pogg.  127.  45.) 

Magnesium  oxide,  MgO. 

Sol.  in  50,000-100,000  pts.  H2O  (Bineau,  C.  R.  41. 
510) ;  in  55,368  pts.  cold  or  hot  H2O  (Fresenius,  A.  59. 
123) ;  in  100,000-200,000  pts.  H2O  (Bunsen) ;  in  16,000 
pts.  H2O  at  ord.  temp.  (Dalton) ;  in  7900  pts.  H2O  at 
ord.  temp.  (Kirwan) ;  in  5760  pts.  H2O  at  15.5°,  and 
36,000  pts.  at  100°  (Fyfe). 


MAGNESIUM  OXYSULPHIDE 


477 


Calc.  from  electrical  conductivity  of  MgO 
+Aq.  1  pt.  MgO  is  sol.  in  172,000  pts.  H2O 
at  18°.  (Dupre",  Zeit.  angew.  Ch.  1903, 16.  55.) 

"Heavy"  MgO  is  more  sol.  in  H2O  than 
"light"  MgO.  The  temp,  of  preparation 
affects  the  rate  of  solution,  the  rate  being 
diminished  as  the  temp,  of  preparation  is 
increased.  (Anderson,  Chem.  Soc.  1905,  87. 
265.) 

Easily  sol.  in  acids,  even  in  H2SO3+Aq. 

Solubility  in  P2O5+Aq  at  25°. 


Composition  of  the 
solution 

*» 

Solid  phase 

G.  MgO 
perl. 

G.  P205 

perl. 

0.207 

0.486 

• 

0.280 

0.732 

0.553 

1.917 

1.438 

4.85 

2.23 

7.35 

1^006 

4.73 

16.84 

1.017 

11.19 

38.59 

1.042 

17.33 

61.21 

1.069 

26.09 
37.40 
75.5 

93.09 
130.7 

281.8 

1.109 
1.144 
1.285 

MgHP04, 
3H20 

109.5 

439.0 

122.6 

498.4 

1.470 

129.9 

546.5 

140.0 

584.0 

146.8 

623.3 

l!595 

147.3 

625.9 

150.3 

645.8 

155.5 

680.7 

87.1 
77.1 

779.6 
809.6 

l'.626 
1.644 

MgH4(P04)2, 

70.6 

835.1 

1.654 

. 

x    2 

(Cameron,  J.  phys.  Chem.  1907,  11.  364.) 

Sol.   in   NH4   salts,    NaCl,   or   KCl+Aq. 

(Fresenius.) 

Solubility  in  MgCl2+Aq  at  25°. 


%  MgCU 

%  MgO  as  Mg(OH)2 

2.36 

0.00008 

4.47 

0.00028 

6.79 

0.00048 

9.02 

0.00080 

13.14 

0.00115 

15.15 

0.00195 

17.53 

.      0.00240 

18.52 

0.00250 

22.04 

0.00245 

23.78 

0.00235 

25.13 

0.00230 

26.88 

0.00250 

28.34 

0.00230 

29.80 

0.00240 

30.04 

0.00250 

34.22 

0.0030 

(Robinson,  J.  phys.  Chem.  1909,  13.  676.) 

More  sol.  in  K2SO4,  and  Na2SO4+Aq  than 
in  H2O.  (Warrington.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

Sol.  in  methyl  alcohol  to  form  a  colloidal 
solution  containing  1.6%  MgO.  (Neuberg 
and  Rewald.  (Biochem.  Z.  1908,  9.  547.) 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1904,  37.  3602.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Insol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

Solubility  in  (calcium  sucrate+ sugar)  + 
Aq. 

1  1.  solution  containing  418.6  g.  sugar  and 
34.3  g.  CaO  dissolves  0.30  g.  MgO;  contain- 
ing 296.5  g.  sugar  and  24.2  g.  CaO  dissolves 
0.24  g.  MgO;  containing  174.4  g.  sugar  and 
14.1  g.  CaO  dissolves  0.22  g.  MgO.  (Boden- 
bender,  J.  B.  1865.  600.) 

See  also  Magnesium  hydroxide. 

Min.  Periclasite. 

Magnesium  peroxide,  MgO2. 

Sol.  in  14,550  pts.  H2O  at  20°.  (Foregger 
and  Philipp,  J.  Soc.  Chem.  Ind.  1906,  26. 
298.) 

5MgO,2MgO2+3H2O. 

3MgO,  2MgO2+3H2O. 

2MgO,2MgO2+3H2O. 

4MgO,2MgO2+3H2O. 

Above  salts  are  decomp.  by  H2O. 

(Carrasco,  Gazz.  ch.  it.  1909,  39,  (1)  47.) 

Magnesium  oxybromide,  MgBr2,  3MgO  -f 

12H20. 

Decomp.  in  the  air  and  also  by  H2O,  al- 
cohol and  most  reagents.  (Tassilly,  C.  R. 
1897,  126.  607.) 

Magnesium  oxychloride,  Mg2OCl2  +  16H2O. 

Easily  decomp.  by  H2O  and  alcohol. 
(Andre,  A.  ch.  (6)  3.  80.) 

+6H2O.    (Andre.) 

2MgO,  HC1,  5H2O  or  3MgO,  MgCl,+ 
10H2O.  Solubility  determinations  show  that 
this  salt  is  the  solid  phase  in  equilibrium  at 
25°  with  solutions  of  MgCl2  and  MgO  con- 
taining from  10-15%  MgCl2.  (Robinson,  J. 
phys.  Chem.  1909,  13.  677.) 

Mg6O5Cl2+6,  8,  14,  or  17H2O.  Decomp. 
by  H2O,  which  dissolves  out  MgCl2.  (Ben- 
der, B.  3.  932.) 

MgnO10Cl2+14,  or  18H2O.  (Krause,  A. 
166.  38.) 

Mg,oO9Cl2  +  24H2O  =  9MgO,  MgCl2  + 
24H2O.  H2O  removes  all  MgCl2  by  long  di- 
gesting. (Bender,  A.  159.  341.) 

+  10,  and  15H2O.    (Bender.) 

Magnesium  oxysulphide,  Mg2OS. 
(Reichel,  J.  pr.  (2)  12.  55.) 


478 


MAGNESIUM  PHOSPHIDE 


Magnesium  phosphide,  Mg3P2. 

Decomp.  by  H2O,  dil.  HCl+Aq,  or  HNO3 
+Aq.  (Parkinson,  Chem.  Soc.  5.  (2)  125  and 
309.) 

Insol.  in  moderately  dil.  cold  HCl+Aq,  or 
boiling  dil.  H2SO4+Aq.  Difficultly  and 
slowly  sol.  in  aqua  regia.  (Blunt,  Chem.  Soc. 
3.  (2)  106.) 

Decomp.  by  H2O,  HC1,  cone.  H,SO4  and 
by  HXO3.  (Gautier,  C.  R.  1899,  128.  1169.) 

Magnesium  silicide,  MgsSi3. 

Slowly  decomp.  by  warm  H2O.  Slowly 
decomp.  by  cold,  rapidly  by  hot  NH4Cl+Aq. 
Decomp.  by  cold  dil.  HCl+Aq.  (Geuther,  J. 
pr.  95.  425.) 

MgsSi.  Decomp.  by  HCl+Aq  with  residue 
of  Si.  (Wohler,  A.  107.  113.) 

Slowly  decomp.  by  H2O  at  ord.  temp. 
Violently  decomp.  by  HC1.  (Lebeau  and 
Bossuet,  C.  R.  1908,  146.  284.) 

Magnesium  sulphide,  MgS. 

Decomp.  by  H2O.  (Rachel,  J.  pr.  (2)  12. 
55.) 

SI.  sol.  in  H2O  with  rapid  decomp.   (Fremy.) 

Sol.  in  acids  with  decomp. 

Anhydrous.  Crustattine.  Only  very  si. 
sol.  in  cold  H2O.  Sol.  in  HNO8  and  HjSO4  at 
ord.  temp.  Sol.  in  PCls  and  in  chromyl  chlor- 
ide. (Mourlot,  C.  R.  1898,  127.  182.) 

Magnesium  poZysulphide,  MgSj. 
Known  only  in  solution.    (Rachel.) 

Magnus'  green  salt. 

See  Platcxftamine  chloroplatmite. 

Manganese,  Mn. 

Decomposes  H2O  even  in  the  cold,  more 
rapidly  when  hot.  (Regnault.) 

Decomposes  cold  water  violently.  (Bun- 
sen.) 

Sol.  in  all  dil.  acids.  Slowly  sol.  in  cold 
HjjSO,.  (John.) 

Insol.  in  cold,  but  rapidly  sol.  in  hot  H2SO4. 
Very  easily  sol.  in  dil.  HzSO4,  or  HCl+Aq, 
HNO3,  or  HC2H3O2+Aq.  (Brunner.) 

Pure  manganese  is  unaltered  in  dry  air, 
even  when  finely  powdered.  Slowly  attacked 
by  cold,  quickly  by  hot  H2O.  Very  si.  at- 
tacked by  cold  H2SO4,  rapidly  on  warming; 
rapidly  attacked  by  cold  dil.  H2SO4+Aq; 
violently  by  cone.  HNO3+Aq;  and  rapidly 
by  dil.  HN03,  HC1,  HC2H3O2+Aq,  and  also 
NaOH+Aq.  Sol.  in  NH4Cl+Aq.  (Pre- 
linger,  W.  A.  B.  102,  2b.  359.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 

^2  ccm.  oleic  acid  dissolves  0.0276  g.  Mn 
in  6  days.  (Gates,  J.  phys.  Chem.  1911,  15. 
14o.) 


Manganese  antimomde,  MnSb. 

Sol.  in  hot  aqua  regia.  (Wedekind,  B. 
1907,  40.  1266.) 

Manganese  azoimide,  basic,  Mn(OH)N3. 

Only  si.  sol.  in  H2O  with  decomp.  (Cur- 
tius,  J.  pr.  1898,  (2)  58.  293.) 

Manganese  bismuthide,  MnBi. 

Very  sensitive  towards  acids  with  the 
exception  of  cone.  HC1.  (Wedekind,  B. 
1911,  44.  2665.) 

Manganese  boride,  MnB. 

Attacked  by  cold  H2O  and  by  acids.  ( Jas- 
soneix,  C.  R.  1904,  139.  1210.) 

Easily  attacked  by  HC1,  H2SO4  and  HF 
with  evolution  of  BH3.  (Wedekind,  B.  1905, 
38.  1231.) 

MnB2.  Sol.  in  acids,  with  evolution  of  H2. 
(Troost  and  Hautefeuille,  A.  ch.  (5)  9.  65.) 

Slowly  decomp.  by  H2O.  Sol.  in  dil.  HC1 
and  other  dil.  acids  with  evolution  of  BH3. 
(Wedekind,  B.  1905,  38.  1229.) 

Manganous  bromide,  MnBr2. 

Anhydrous.    Very  deliquescent. 

Sat.  MnBr2+Aq  contains  at: 
—21°  +7°     11°      18°      38°      52° 

52.1  56.5    57.0    59.1    62.7    64.2%  MnBr2, 

64°     76°     89°     97°     105° 

68.2  70.1    69.7    69.2    70.2%  MnBr2. 

(fitard,  A.  ch.  1894,  (7)  2.  541.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

+H,O.    (Lescoeur,  A.  ch.  1894,  (7)  2. 104.) 

+4H2O.  More  deliquescent  than  MnCl2. 
Melts  in  crystal  water  when  heated.  (Berthe- 
mot.) 

+6H20.    (Kuznetzoff,  C.  C.  1897,  II.  329.) 

Manganous  mercuric  bromide. 
Deliquescent. 

Manganous  palladium  bromide. 
See  Bromopalladite,  manganous. 

Manganous  stannic  bromide. 
See  Bromostannate,  manganous. 

Manganese  carbide,  MnC. 

(Brown,  J.  pr.  17.  492.) 

MnC2. 

Mn3C.  (Troost  and  Hautefeuille,  A.  ch. 
(5)  9.  60.) 

Decomp.  by  H2O  and  by  dil.  acids.  (Mois- 
san,  C.  R.  1896,  122.  422.) 

Manganous  chloride,  MnClz. 
Anhydrous.    Deliquescent. 


MAXGAXOUS  CHLORIDE 


479 


100  pts.  H2O  at  t°  dissolve  pts.  MnCl2: 


Pts.  MnCl2 


Pts.  MnCU 


Sp.  gr.  of  MnCl2+Aq  at  room  temp. 


MnCl2 


Sp.  gr. 


10 

31.25 

62.5 


62.16 

85.72 

122.22 


87.5 
106.25 


122.22 
123.81 


or,  sat.  MnCl2+Aq  at  t°  contains: 


8.007 
15.650 
30.330 
40.132 


1.0960 
1.1963 
1.3372 
1.4530 


t° 

%  MnClz 

t° 

%  MnCU 

10 
31.25 
62.5 

38.33 
46.15 
55.0 

87.5 
106.25 

55.0 
55.32 

(Wagner,  W.  Ann.  1883,  18.  273.) 


Sp.  gr.  of  MnCl2+Aq  at  t' 


(Brandes,  Pogg.  22.  263.) 
See  also  below  under  +2H2O,  and  +4H2O. 

Sp.  gr.  of  MnCl2+Aq  at  15°.  a=sp.  gr.  if  % 
is  MnCl2;  b=sp.  gr.  if  %  is  MnCl2+ 
4H20. 


t° 

%  MnCli 

Sp.  gr. 

14.5 
14.5 
14.0 
14.5 
14.0 
14.6 

5.0 
11.99 
14.98 
19.92 
23.10 
28.51 

1.0457 
1.1076 
1.1379 
1.1891 
1.2246 
1.2888 

5 
10 
15 
20 
25 
30 
35 


1.045 
.091 
.138 
.189 
.245 
.306 

1.372 


1.0285 

1.057 

1.086 

1.116 

1.147 

1.180 

1.214 


40 
45 
50 
55 
60 
65 
70 


1.443 
1.514 


1.250 
.290 
.331 
.375 
.419 
.463 
.508 


(Long,  W.  Ann.  1880,  11.  38.-) 
Sp.  gr.  of  MnCl2+Aq  at  25°. 


Concentration  of  MnClz  +Aq 


1-normal 

Vr-     " 
V<-     " 

Vr-      " 


Sp.  gr. 


1.0513 
1.0259 
1.0125 
1.0063 


(Gerlach,  Z.  anal.  28.  476.)  (Wagner,  Z.  phys.  Ch.  1890,  5.  38.) 

Solubility  of  MnCl2+KCl  in  H»O  at  t°. 


t° 

%  MnCl. 

%KC1 

Solid  phase 

6 

40.23 
35.94 

9^41 
23.06 

MnCl2,  4H2O 
MnCl2,  4H20+MnCl2,  KC1,  2HSO+KC1 
KC1 

28.4 

44.46 
43.28 
38.65 

8^66 
13.79 

26.91 

MnCl2,  4H2O 
MnClj,  4H2O+MnCl2,  KC1,  2H,O 
MnCl2,  4H,0+MnCl2,  2KC1,  2H2O+KC1 
KC1 

52.8 

50.14 

6.01 

MnCl2,  4H2O+MnCl2,  2H2O+MnCl2,  KC1,  2H2O 

62.6 

51.86 
49.95 
44.05 
36.85 

6".67 
12.49 
18.77 
31.57 

MnCl2,  2H20 
MnCl2,  2H20+MnCl2,  KC1,  2H2O 
MnCl2,  KC1,  2H20+MnCl2,  2KC1,  2H2O 
MnCl2,  2KC1,  2H2O+MnCl2,  4KC1 
KC1 

(Suss,  Z.  Kryst.  Min.  1912,  51.  262.) 


Insol.  in  liquid  XH3.     (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 


Solutions  of  MnCl2  in  75%  alcohol  saturated 
at  t°  contain: 


t° 

%  MnCU 

t 

%  MnCli 

10 
25 

23.1 
36.1 

43.75 

87.5 
(B.-pt.) 

37.5 
32.2 

480 


MANGANESE  CHLORIDE 


Solutions  of  MnCl2  in 
rated  at  t 

absolute  alcohol  satu- 
0  contain: 

Sat.  aq.  solution  contains  at: 
—22°    —5°    +7°      17°      19° 
34.7      37.8    40.4    41.2     42.3%  MnCl2 

35°      55°      57°      80°     100°     140° 
44.4    48.2    50.0    51.0    53.7   54.7%  MnCl2. 
(fitard,  A.  ch.  1894,  (7)  2.  537.) 

Solubility  in  H2O  at  t°. 

t° 

%  MnCl2 

t° 

%  MnCl2 

11.25 
37.5 

33.3 
33.3 

76.25 
(B.-pt.) 

36.2 

(Brandes,  I.  c.) 

MnCl2  crystallises  from  above  solutions  on 
standing. 
When  15-20  vols.  ether  are  added  to  1  vol. 
absolute  alcohol  sat.  with  MnCl2,  MnCl2  is 
completely  pptd.    (Dobereiner.) 
Insol.  in  oil  of  turpentine. 
Sol.  in  urethane.    (Castoro,  Z.  anorg.  1899, 
20.  61.) 
SI.   sol.   in  .benzonitrile.      (Naumann,    B. 

t 

Pts.  MnCh  per 
100  pts.  H2O 

Sp.  gr.  of  sat. 
solution 

25 
30 
40 
50 
*57.65 

77.18 

80.71 
88.59 
98.15 
105.40 

1.4991 
1.5049 
1.5348 
1.5744 
1.6097 

1914,  47.  1369.) 

Difficultly  sol.  in  methyl  acetate.  (Nau- 
mann, B.  1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910.  43.  314.) 

+H2O.  Solubility  in  HCl+Aq  decreases 
with  increasing  amt.  of  HC1.  It  is  greater 
when  hot  than  cold,  but  is  not  inconsiderable 
even  when  HC1  is  cone.  1  1.  cone.  HCl+Aq 
sat.  at  12°  dissolves  190  g.  MnCl2  from  MnCl2 
+H2O.  (Ditte,  C.  R.  1881,  92.  243.) 

+5/3H2O.  MnCl2+4H2O  effloresces  to 
MnCla+VsHaO  in  a  dry  atmosphere  and 
under  low  pressure  and  not  to  MnCl2+ 
2H2O.  (Sabatier,  Bull.  Soc.  1894,  (3)  11. 
547.) 


+2H20. 


Solubility  in  H2O  at  t°. 


60 
70 
80 


Pts.  MnCl2  per 
100  pts.  H2O 


108.6 

110.6 
112.7 


Sp.  gr.  of  sat. 
solution 


1.6108 
1.6134 


(Dawson  and  Williams,  Z.  phys.  Ch.  1899, 
31.  63.) 

Sat.  aqueous  solution  of  MnCl2+2H2O. 
Contains  51.86%  MnCl2  at  62.6°.  (Suss.  Z. 
Krist.  1912,  61.  262.) 

+4H2O.    Deliquescent. 

100  pts.  H20  at  t°  dissolve: 


t° 

Pts.  MnCh 
+4H2O 

t° 

Pts.  MnCh 
+4H20 

8 
31.25 
62.5 

151 
265 
641 

87.5 
106.25 

641 
656 

(Brandes,  I.  c.) 

Sol.  in  0.8  pt.  H2O  at  18.75°.    (Abl.) 
Pptd.  from  solution  in  9.17  mols. 
(Kuznetzoff,  C.  C.  1899,  I.  246.) 


H2O 


*Temp.  of  transition  into  MnCl2+2H2O. 

(Dawson  and  Williams,  Z.  phys.  Ch.  1899,  31. 

63.) 

Sat.  aqueous  solution  of  MnCl2+4H2O 
contains  40.23%  MnCl2  at  6°;  44.6%  MnCl2 
at  28.4°.  (Sites,  Z.  Krist.  1912,  51.  262.) 

100  pts.  75%  alcohol  dissolve  at  t°: 


10 
25 


Pts.  MnCh 
+4H20 


53 
132 


43.75 

87.5 


Pts.  MnCl2 
+4H2O 


144 
100. 


(Brandes,  I.  c.) 

Insol.  in  absolute  ether,  which  also  does 
not  abstract  crystal  H2O. 

Insol.  in  boiling  oil  of  turpentine.  (Brandes. 

Sol.  in  cone.  HNO3+Aq. 

+5H2O.  (Muller-Erzbach,  B.  1889,  22. 
3181.) 

+6H2O.  Pptd.  from  solution  in  11.7  mols. 
H2O  at  —21°.  (Kuznetzoff,  C.  C.  1899,  I. 
246.) 

Manganese  ^nchloride,  MnCl3. 

Immediately  decomp.  by  H2O;  sol.  in  abs. 
ether  and  in  abs.  alcohol.  (Holmes,  J.  Am. 
Chem.  Soc.  1907,  29.  1285.) 

Manganese  teZrachloride,  MnCl4. 

Has  not  been  isolated. 

Sol.  in  H2O,  alcohol,  or  ether.  (Nickles, 
J.  B.  1866.  225.) 

Composition  is  Mn2Cl6.  (Christensen,  J. 
pr.  (2)  34.  41.) 

Manganese  hydrogen  tetraddoride   (chloro- 

manganic  acid),  MnCl4,  2HC1. 
Sol.  in  ether;  decomp.  by  H2O.     (Franke, 
(2)  36.  31.) 

Manganese  Tieptachloride,  MnCl7(?). 

Decomp.  by  H->O.  (Dumas,  Berz.  J.  B.  7. 
112.) 


MANGANIC  SODIUM  FLUORIDE 


481 


Has  the  formula  MnO3Cl  (?).  (Aschoff,  J. 
pr.  81.  29.) 

Manganous  mercuric  chloride,  MnCl2,  HgCl2 
+4H20. 

Deliquescent  in  moist  air.  Easily  sol.  in 
H2O.  (v.  Bonsdorff.) 

MnCl2,  2HgCl2.  (Varet,  C.  R.  1896,  123, 
422.) 

Manganous  potassium  chloride,  MnCl2,  KC1 
+2H2O. 

Deliquescent.  Very  sol.  in  H2O,  but  is 
decomp.  thereby.  (Remsen  and  Saunders, 
Am.  Ch.  J.  14.  129.) 

MnCl2,  2KC1+2H2O.  (Suss,  Z.  Kryst. 
1912,  51.  262.) 

Manganic  potassium  chloride,  MnCls,  2KC1+ 

H2O. 
Decomp.  by  H2O.    Sol.  in  HC1  apparently 


without  decomp.     (Rice,  Chem. 
73.  261.) 


>c.  1898, 


MnCl4,     2KC1.       Very     easily     decomp. 
(Meyer  and  Best,  Z.  anorg.  1899,  22.  186.) 


nC!4,    MnCl3,    5KC1.      Easily    decomp. 
(Meyer  and  Best,  Z.  anorg.  1899,  22.  185.) 

Manganous  rubidium  chloride,  MnCl2, 
2RbCl. 

(Godeffroy.) 

+3H2O.  Easily  sol.  in  H2O.  Insol.  in 
alcohol;  cone.  HCl+ppt.  anhydrous  salt 
from  aqueous  solution.  (Godeffroy,  Arch. 
Pharm.  (3)  12.  40.) 

Contains  only  2H2O.  (Saunders,  Am.  Ch. 
J.  14.  139.) 

Manganous  thallic  chloride,  MnCl2,  2T1C13  + 

6H2O. 

Can  be  cryst.  from  H2O.  (Gewecke,  A. 
1909,  366.  224.) 

Manganous  stannic  chloride. 
See  Chlorostannate,  manganous. 

Manganous  chloride  hydrazine,   MnCl2, 

2N2H4. 
Ppt.    (Franzen,  Z.  anorg.  1908,  60.  285.) 

Manganous  chloride  hydroxylamine.  MnCl2, 

2NH2OH. 

Very  stable:  insol.  in  alcohol.  (Feldt,  B. 
1894,  27.  405.) 

Manganous  fluoride,  MnF2. 

Only  sol.  in  H2O  containing  HF.  (Ber- 
zelius.) 

Insol.  in  H2O;  decomp.  by  boiling  with 
H2O;  si.  sol.  in  liquid  NH3;  easily  sol.  in  cold 
or  hot  cone.  HNO3  and  HC1;  slowly  sol  in 
dil.  HC1;  decomp.  by  fused  K2CO8,  KOH, 
KNO3,  and  KC1O3;  insol.  in  alcohol  and 


ether.  Slowly  sol.  in  acetic  acid.  (Moissan, 
C.  R.  1900,  130.  1160.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Manganese  Znfluoride,  MnF3. 

Completely  sol.  in  a  little  H2O,  but  decomp. 
by  dilution  or  boiling.  (Berzelius.) 

-H>H2O.  Efflorescent.  (Christensen,  J.  pr. 
(2)  35.  57.) 

Sol.  in  H2SO4,  HC1,  HNO3;  decomp.  by 
H20;  insol.  in  most  organic  solvents.  (Mois- 
san, C.  R.  1900,  130.  626.) 

Manganomanganic  fluoride,  Mn3F8+10H2O. 
Sol.  in  a  little  H2O,  but  decomp.  by  dilu- 
tion.   (Nickles,  C.  R.  67.  448.) 

Manganese  tefrafluoride,  MnF4. 

Not  isolated.  Sol.  in  absolute  alcohol  or 
ether;  decomp.  by  H2O.  (Nickles,  C.  R.  65. 
107.) 

Probably  does  not  exist.  (Christensen,  J. 
pr.  (2)  35.  161.) 

Manganese  Aeptafluoride,  MnF7  (?). 
Sol.  in  H2O  with  decomp.    (Wohler.) 

Manganese  sesquiftuoride  with  MF. 
See  also  Fluomanganate,  M. 

Manganic  nickel  fluoride,  2NiF2,   Mn2F6+ 

8H2O. 
(Christensen,  J.  pr.  (2)  34.  41.) 

Manganic  potassium  fluoride,  Mn2F6,  4KF+ 
2H20. 

Decomp.  by  H2O.  Sol.  in  cone.  HCl+Aq, 
dil.  HNO3+Aq,  cone.  H2SO4+Aq,  H3PO4+ 
Aq,  H2C2O4+Aq,  H2C4H4O6  +  Aq,  and  dil. 
HF+Aq.  (Christensen,  J.  pr.  (2)  35.  72.) 

MnF4,  2KF.  Difficultly  sol.  in  H2O.  De- 
comp. by  much  H2O.  (Nickles,  C.  R.  65. 
107.) 

True  composition  is  Mn2F6,  4KF,  also  with 
2H2O.  (Christensen,  J.  pr.  (2)  34.  41.) 

MnF4,  4KF.    (Nickles.) 

See  also  Fluomanganate,  potassium. 

Manganic  rubidium  fluoride. 
See  Fluomanganate,  rubidium. 

Manganic   silver   fluoride,   2AgF,    Mn2F6+ 

14H2O. 
Sol.  in  HF+Aq.     (Christensen,  J.  pr.  (2) 

Manganic  sodium  fluoride,  Mn2F6,  4NaF. 

Decomp.  by  much  H2O.  Not  as  sol.  in  HF 
+Aq  as  the  K  salt.  (Christensen,  J.  pr.  (2) 
35.  161.) 


482 


MANGANOMANGANIC  THALLOUS  FLUORIDE 


Manganomanganic  thallous  fluoride,  5T1F, 
2MnF3,  MnF2. 

Decomp.  by  H2O. 

SI.  sol.  in  dil.,  easily  sol.  in  cone.  HF. 

Sol.  in  cone.  HC1,  dil.  HNO3,  and  cold  or 
hot  cone.  H2SO4. 

Sol.  in  warm  H2O2  containing  H2S04. 

Sol.  in  dil.  tartaric  and  oxalic  acids. 
(Ephraim,  B.  1909,  42.  4458.) 

Manganous  stannic  fluoride. 
See  Fluostannate,  manganous. 

Manganic  zinc  fluoride,  2ZnF2,  Mn2F6+8H2O 
See  Fluomanganate,  zinc. 

Manganous  zirconium  fluoride. 
See  Fluozirconate,  manganous. 

Manganous  fluoride  ammonia,  3MnF2,  2NH3. 
(Moissan,  C.  R.  1900,  130.  1161.) 

Manganous  hydroxide,  MnO2H2. 

2.15  x  10-5  g.-mol.  are  sol/,  in  1 1.  H2O  at  18°. 
(Sackur,  Z.  Elektrochem,  1909,  15.  846.) 

Solubility  in  H2O  =0.6  x  10~4  g.  mol.  (Herz, 
Z.  anorg.  1899,  22.  284.) 

1  1.  H2O  dissolves  2  x  10~4  mol.  MnO2H2. 
(Tamm,  Z.  phys.  Ch.  1910,  74.  500.) 

Very  si.  sol.  in  H2O  or  alkalies.  (Fresen- 
ius.)  Easily  sol.  in  acids.  Insol.  in  NaOH, 
orKOH+Aq.  Sol.  in  NH4  salts +Aq.  Insol. 
in  NH4OH+Aq.  Sol.  in  NaOH+Aq  in 
presence  of  glycerine.  (Donath,  Dingl.  229. 


Not  pptd.  by  NH4OH+Aq  in  presence  of 
H2C4H4Oe;  by  KOH+Aq  in  presence  of  cane 
sugar;  by  KOH+Aq  in  presence  of  Na  citrate. 

Solubility  of  MnO2H2  in  organic  Na  salts + 
Aq.  (0.5  normal.) 

Na  tartrate,  0.0068  mol.  per  1. 

Na  malate,  0.0042       "      "   " 

Na  citrate,  0.0126       "      "   " 

(Tamm,  Z.  phys.  Ch.  1910,  74.  496.) 

Min.  Pyrochroite. 

Manganomanganic  hydroxide,  Mn3O4,  #H2O. 
Not  attacked  by  boiling  NH4Cl+Aq.    Be- 
haves towards  acids  as  Mn2O3. 

Manganic  hydroxide,  Mn2O3,  H2O. 

Insol.  in  hot  or  cold  dil.  H2SO4+Aq. 

Sol.  in  cone.  H2SO4  at  somewhat  over  100°. 
<Carius.) 

Sol.  in  tartaric,  oxalic,  and  malic  acids,  with 
subsequent  decomp.  Insol.  in  formic,  acetic, 
benzoic,  or  hippuric  acids.  (Hermann,  Pogg. 
74.  303.) 

Insol.  in  NH4Cl+Aq.  Insol.  in  cane  sugar 
-f  Aq.  (Peschier.) 

Min.  Manganile.  Sol.  in  cone.  HCl-f-Aq. 
SI.  sol.  in  cone.  H2SO4. 


Manganese  efohydroxide,  MnO2,  H2O. 
See  Manganous  acid. 

Manganous  iodide,  MnI2. 

Anhydrous.  Nearly  insol.  in  AsBr3. 
(Walden,  Z.  anorg.  1902,  2fc  374.) 

Sol.  in  POC13.  (Walden,  Z.  anorg.  1900, 
25.  212.) 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  828.) 

+4H2O.  Very  deliquescent,  and  sol.  in 
H2O.  (Kuznetzoff,  C.  C.  1900,  II.  525.) 

+9H2O.    (Kiuznetzoff.) 

Manganous  mercuric  iodide,  MnI2,  2HgI2-f 
6H2O. 

Decomp.  by  H2O.  Sol.  without  decomp. 
in  alcohol  and  acetone.  (Dobroserdoff,  C.  C. 
1901,  I.  363.) 

3MnI2,  5HgI2+20H2O. 

A  sat.  solution  in  H2O  at  17°  has  composi- 
tion 1.4  MnI2,  HgI2+ 10.22  H2O  and  sp.  gr.  = 
2.98.  (Duboin,  C.  R.  1906,  142.  1338.) 

Very  sol.  without  decomp.  in  methyl,  pro- 
pyl,  isopropyl,  isobutyl,  and  allyl  alcohols, 
ethyl  acetate  and  ethyl  cyanide.  Somewhat 
less  sol.  in  amyl,  propyl  and  isobutyl  ace- 
tates, acetone,  acetic  acid,  formic  acid  (with 
ppnt.  of  HgI2),  ethyl  benzoate,  ethyl  oxalate, 
butyl  alcohol,  amyl  alcohol  and  nitrobenzene. 
SI.  decomp.  by  glycerine.  Insol.  in  ethyl  ni- 
trate, ethylene  bromide,  toluene,  benzene, 
CHC13,  CC14,  ethyl  iodide,  monobrom-  and 
monochlorbenzene.  (Duboin,  A.  ch.  1909, 
(8),  16.  278.) 

Manganese  nitride,  Mn3N2. 

Sol.  in  HNO3  only  on  heating.  HCl+Aq 
dissolves  only  in  presence  of  Pt.  Aqua  regia 
dissolves  slowly.  H2SO4  acts  only  when  hot 
and  cone.  Insol.  in  acetic  acid.  (Prelinger, 
M.  1894,  15.  398.) 

Mn5N2.  Sol.inNH4Cl+AqandNH4OH+ 
Aq;  insol.  in  HC1;  sol.  in  HNO3+Aq.  with 
decomp.  (Prelinger,  M.  1894,  15.  398.) 

Mn7N2.  Easily  attacked  by  acids  and  al- 
kalies. (Wedekind,  B.  1908,  41.  3772.) 

Manganous  oxide,  MnO. 

Insol.  in  H2O.  Easily  sol.  in  acids.  Readily 
sol.  in  NH4Cl+Aq. 

Manganic  oxide  (Manganese  ses<?m'oxide), 
Mn2O3. 

Decomp.  by  boiling  with  HNO3+Aq  into 
MnO,  which  dissolves,  and  MnO2,  which  is 
insol.  (Berthier);  also  by  boiling  with  dil. 
H2SO4+Aq.  (Turner.)  Sol.  in  hot  cone. 
H2SO4  or  HCl+Aq.  Sol.  in  cold  HCl+Aq 
without  decomp.  If  perfectly  pure,  is  insol. 
in  dil.  H2S04+Aq,  but  if  it  contains  any 
MnO,  it  dissolves.  (Rose.)  Insol.  in  boiling 
NH4Cl+Aq. 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 


MANGANOUS  PHOSPHOSELENIDE 


483 


Solubility  in  (calcium  sucrate-f- sugar)  + 
Aq. 

1  1.  solution  containing  418.6  g.  sugar  and 
34.3  g.  CaO  dissolves  0.50  g.  Mn2O3;  contain- 
ing 296.5  g.  sugar  and  24.2  g.  CaO  dissolves 
0.37  g.  Mn2O3;  containing  174.4  g.  sugar  and 
14.1  g.  CaO  dissolves  0.32  g.  MnoO3.  (Boden- 
bender,  ,1.  B.  1865.  600.) 

Min.  Braunite. . 

Colloidal.  Solution  in  H2O  containing  0.21 
g.  to  a  litre  is  precipitated  by  KNO3+Aq 
(1  : 1000);  K2SO4+Aq  (1  :  1100);  (NH4)2SO4 
+Aq  (1  : 1500);  NaCl+Aq  (1  :  1580);  MgSO4 
+Aq  (1:40,983);  BaCl2+Aq  (1:58,823); 
MnSO4+Aq  (1  : 147,929);  (NH4)2A12(SO4)4  + 
Aq  (1  : 362,318);  K2Cr9(S04)4+Aq  (1  :  416, 
HCl+Aq  (1:61,350);  HC2H3O2  (1  : 


17,262);  H2SO4  (1  :  62,500).     (Spring  and  de 
Boeck,  Bull.  Soc.  (2)  48.  170.) 

Manganomanganic  oxide,  Mn3O4. 

Insol.  in  H2O.  Boiling  dil.  or  cone.  HNO3  + 
Aq  dissolves  out  MnO  (Berthier) ;  also  boiling 
dil.  H2SO4+Aq.  (Turner.)  Sol.  in  hot  HC1 
+Aq.  (Otto.)  NH4Cl+Aq  dissolves  out 
MnO.  (Rose.)  Sol.  without  decomp.  in  hot 
very  cone.  H3PO4+Aq,  and  cold  cone.  H2SO4, 
HC1,  oxalic,  and  tartaric  acids +Aq. 

Min.  Hausmannite. 

Manganese  dioxide,  MnO2. 

Min.  Pyrolusite.  Tnsol.  in  H2O.  Very 
slowly  sol.  in  cone.  H2SO4  with  evolution  of 
O2.  Sol.  in  cold  HCl+Aq;  decomp.  by  hot 
HCl+Aq.  Sol.  in  aqua  regia.  Sol.  in  SO2  + 
Aq  or  N2O3+Aq.  (Karsten.) 

Insol.  in  HNO3,  or  dil.  H2SO4+Aq,  except 
in  presence  of  organic  reducing  substances. 
Decomp.  by  citric  acid,  and  more  easily  by 
oxalic  acid.  (Bolton.) 

SI.  sol.  in  hot  cone.,  but  insol.  in  dil.  HNO3 
+Aq.  (Deville.)  When  pure  it  is  insol.  in 
cold  dil.  H2SO4+Aq,  but  if  a  small  quantity 
of  MnO  is  added  much  MnO2  dissolves. 
(Carius.) 

Not  decomp.  by  boiling  NH4Cl+Aq. 

Easily  sol.  in  a  mixture  of  nitrososulphuric 
acid  and  cone.  HCl+Aq.  (Borntrager,  Rep 
anal.Ch.  1887.  741.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Manganese  oxides,  Mn3O5,  Mn6On,  etc. 
See  Manganite,  manganous. 

Manganese  ^n'oxide,  MnO3. 

Deliquescent.  Sol.  in  H2O,  with  subse- 
quent decomp.  Decomp.  by  ether.  Sol.  in 
cone.  H2SO4.  (Franke,  J.  pr.  (2)  36.  31.) 

Manganese  ^roxide,  MnO4  (?). 

SI.  sol.  in  H2O  with  decomp.  Decomp.  b} 
H2SO4  or  ether.  (Franke,  J.  pr.  (2)  36.  166. 


Manganese  heptoxide,  Mn2O7. 

Very  unstable;  takes  up  H2O  from  air.  Sol. 
n  H2O  with  evolution  of  heat  and  rapid 
[ecomposition.  Sol.  in  cone.  H2SO4  without 
lecomp.  (Aschoff.) 


Manganese  oxychloride,  3Mn2O3,  MnCl2. 
Insol.  in  H2O.    (Saint-Gilles,  C.  R.  55.  329.) 
MnCl2,  MnO  (?).     (Gorgeu,  A.  ch.  (6)  4. 
15.) 
MnO3Cl.    See  Manganyl  chloride. 

Manganic  oxyfluoride,  MnOF2. 
Sol.  in  absolute  ether. 
MnOF2,   2HF  =  fluoxymanganic   acid. 
Nickles,  C.  R.  659.  107:) 


Manganic  oxyfluoride  potassium  fluoride. 
See  Fluoxymanganate,  potassium. 

Manganic  sesgmoxyfluoride  potassium  fluor- 
ide. 
See  Sesquifl.uoxymanga.na.te,  potassium. 


Manganous  oxyiodide,  MnI2,  MnO+6H2O. 

Sol.  in  H2O  with  decomp.     (Kuznetzoff, 
C.  C.  1913, 1.  1659.) 


Manganese  oxysulphide,  MnO,  MnS. 
Sol.  in  acids.    (Arfvedson,  Pogg.  1.  50.) 


Manganese  phosphide,  Mn3P2. 

Insol.  in  dil.  acids;  sol.  in  hot  cone.  HNO3. 
(Wedekind,  B.  1907,  40.  1268.) 

Sol.  in  aqua  regia;  insol.  in  HNO3.  (Grang- 
er, C.  R.  1897,  124.  191.) 

Mn5P2.  HCl+Aq.  dissolves  put  Mn3P2  and 
leaves  Mn7P2,  which  is  sol.  in  HNO3+Aq. 
(Wohler  and  Merkel,  A.  86.  371.) 

Not  attacked  by  boiling  H2O  or  by  HC1. 
Easily  sol.  in  warm  HNO3  or  aqua  regia. 
(Wedekind  and  Veit,  B.  1907,  40.  1268.) 

#Mn3P2, 7/Mn4P2.  Easily  sol.  in  aqua  regia; 
partly  sol.  in  H2S04  or  HCl+Aq.  (Struve,  J. 
pr.  79.  321.) 

Mn6P2.  Insol.  in  HCl+Aq.  Sol.  in  HNO3 
+Aq.  (Schrotter,  W.  A.  B.  1849,  1.  305.) 

Manganous  phosphoselenide,  MnS,  P2Se. 

Insol.  in  H2O.  Sol.  in  HCl+Aq  or  HNO3  + 
Aq.  Insol.  in  cold,  si.  decomp.  by  hot  alkalies 
+Aq.  (Hahn,  J.  pr.  93.  436.) 

2MnSe,  P2Se3.  Insol.  in  cold,  slowly  sol. 
in  hot  HCl+Aq.  Not  decomp.  oy  alkalies. 

2MnSe,  P2Se6.  Easily  decomp.  by  acids. 
(Hahn.) 


484 


MANGANESE  SELENIDE 


Manganese  selenide,  MnSe. 

Decomp.  by  H2O  and  min.  acids.  (Wede- 
kind,  B.  1911,  44.  2667.) 

Cryst.  SI.  decomp.  by  H20  at  100°;  easily 
sol.  in  dil.  acids.  (Fonzes-Diacon,  C.  R.  1900, 
130.  1025.) 

Manganese  silicide. 

Sol.  in  HF;  only  very  si.  sol.  in  other  acids. 
(Warren,  C.  N.  1898,  78.  319.) 

Mg6Si2.  Sol.  in  HCl+Aq  with  evolution 
of  SiH4.  (Wohler,  A.  106.  54.) 

Mn2Si.  Insol.  in  H2O.  (Vigouroux,  C.  R. 
1895,  121.  772.) 

Easily  sol.  in  HF.  (Wedekind,  B.  1911, 
44.  2668.) 

Easily  sol.  in  dil.  acids,  HF  and  HNO3. 
Insol.  in  KOH+Aq.  (Vigouroux,  A.  ch. 
1897,  (7)  12.  179.) 

Easily  sol.  in  HF  when  heated;  in  HC1 
when  red  hot.  Sol.  in  dil.  min.  acids  with 
decomp.  (Vigouroux,  C.  R.  1895,  121. 
772.) 

Insol.  in  HNO3;  sol.  in  dil.  or  cone.  HC1. 
Slowly  decomp.  by  alkali  hydroxides.  (Le- 
beau,  C.  R.  1903,  136.  91.) 

Mn2Si.  Easily  sol.  in  molten  alkali. 
(Vigouroux,  C.  R.  1895,  121.  772.) 

MnSi.  Slowly  attacked  by  hot  cone.  HC1. 
Not  acted  upon  by  dil.  or  cone.  HN03  or 
H2SO4.  (Lebeau,  C.  R.  1903,  136.  91.) 

MnSi2.  Not  attacked  by  HNO3  or  H2SO4. 
Easily  sol.  in  cold  HF;  decomp.  by  cone, 
alkalies +Aq.  (Lebeau,  C.  R.  1903,  136. 
233.) 

Manganous  sulphide,  MnS. 

Anhydrous.  Insol.  in  H2O.  Sol.  in  weak 
acids,  even  in  acetic  acid. 

1  1.  H2O  dissolves  71.60  x  1(H  moles  MnS 
at  18°.  (Weigel,  Z.  phys.  Ch.  1907,  58.  294.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Min.  Alabandite.    Sol.  in  HCl+Aq. 

+  ^H2O.  Green.  Decomp.  by  boiling 
with  H2O.  Sol.  in  weak  acids,  as  acetic  or 
sulphurous  acid.  Very  si.  sol.  m  (NH4)2S  + 
Aq.  (Wackenroder.) 

Sol.  in  NH4  salts +Aq.  100  ccm.  of  sat. 
NH4Cl+Aq  at  12°  dissolve  0.43  g.  MnS. 
(Clermont  and  Guyot,  C.  R.  85.  37.) 

+3/2H2O.  Flesh-colored.  Less  sol.  in  NH4 
salts,  or  acetic  acid+Aq  than  the  preced- 
ing salt.  100  ccm.  of  sat.  NH4C1+ 
Aq  at  12°  dissolve  0.088  g.  (Clermont  and 
Guyot.) 

Neither  green  nor  flesh-coloured  MnS  con- 
tains H2O.  (Antony  and  Donnini,  Gazz.  ch. 
it.  23.  560.) 

MnS  is  not  pptd.  in  presence  of  alkali 
citrates,  tartrates,  or  grape  sugar;  cane  or 
milk  sugar  do  not  prevent  precipitation. 
(Spiller.)  Not  pptd.  in  presence  of  Na4P2O7. 
(Rose.) 


Manganese  sulphide,  Mn3S4. 

Decomp.  by  H2O.  Sol.  in  cold  dil.  acids. 
(Gautier  and  Hallopeau,  C.  R.  1889,  108. 
809.) 

Manganese  cfosulphide,  MnS2. 

(Senarmont,  J.  pr.  51.  385.) 

Min.  Hauerite.  Decomp. -by  hot  HCl+Aq 
with  separation  of  S. 

Manganous  phosphorus  sulphide,  MnS,  P2S. 
Sol.  in  HCl+Aq  with  decomp.    (Berzelius, 
A.  46.  147.) 

Manganous  potassium  sulphide,  3MnS,  K2S. 
Nearly  insol.  in  water,  alcohol,  or  ether. 
Easily  sol.  in  acids.    (Volcker,  A.  59.  35.) 

Manganous  sodium  sulphide,  3MnS,  Na2S. 

Insol.  in  H2O,  alcohol,  or  ether.  Sol.  in 
dil.  acids,  and  SO2+Aq.  (Volcker.) 

2MnS,  Na2S.  Decomp.  by  H2O.  (Schneid- 
er, Pogg.  151.  446.) 

Manganese  telluride,  MnTe. 

Decomp.  by  H2O  and  min.  acids.  (Wede- 
kind, B.  1911,  44.  2667.) 


Manganic  acid,  H2MnO4. 

Known   only   in   solution,    which   decom- 
poses rapidly.     (Franke,  J.  pr.  (2)  36.  31.) 


Barium  manganate,  BaMnO4. 

Insol.  in  H2O;  decomp.  by  acids, 
scherlich.) 


(Mit- 


Didymium  manganate,  Di2(MnO4)3. 

Insol.  in  H2O.  Sol.  in  H2SO4+Aq. 
(Frerichs  and  Smith,  A.  191.  331.) 

Does  not  exist.    (Cleve,  B.  11.  912.) 

Lanthanum  manganate,  La2(MnO4)3. 
Ppt.    (Frerichs  and  Smith,  A.  191.  331.) 
Does  not  exist.    (Cleve,  B.  11.  912.) 

Manganese    manganate,    Mn2O3,    Mn03  = 

3MnO2. 
See  Manganese  dioxide. 

Lead  manganate,  PbMnO4+2H2O. 
Ppt.    (Jolles,  C.  C.  1888.  58.) 

Potassium  manganate,  K2MnO4. 

Sol.  in  water  containing  alkalies  without 
decomp.,  but  decomp.  by  pure  H2O.  Can  be 
recrystallised  from  dil.  KOH+Aq. 


MANGANOCYANHYDRIC  ACID 


485 


Solubility  in  KOH+Aq  at  t°. 

Solvent 

t° 

Mol.  K2MnO4  in 

1  1.  of  sat.  solution 

2-N  KOH 

0 

0.907 

10 

1.013 

20 

1.140 

30 

1.252 

45 

1.424 

4-N  KOH 

0 

0.554 

17 

0.681 

25 

0.733 

30 

0.772 

40 

0.852 

45 

0.889 

51 

0.938 

60 

1.003 

70 

1.074 

80 

1.143 

6-N  KOH 

0 

0.155 

15 

0.224 

23 

0.261 

30 

0.303 

40 

0.362 

45 

0.388 

60 

0.469 

70 

0.528 

80 

0.587 

8-N  KOH 

0 

0.063 

10 

0.070 

20 

0.078 

30 

0.096 

40 

0.119 

50 

0.142 

60 

0.167 

70 

0.196 

80 

0.222 

10-N  KOH 

0 

0.0145 

10 

0.0152 

20 

0.0160 

30 

0.0215 

40 

0.0305 

50 

0.0462 

63 

0.0620 

70 

0.0700 

80 

0.0830 

(Sackur,  Z.  Elektrochem.  1912,  18.  724.) 

Sol.  in  ethyl  acetate.    (Naumann,  B.  1910, 
43.  314.) 

Potassium  manganate  permanganate, 

K2MnO4,  KMnO4. 

Sol.  without  decomp.  in  20%  KOH+Aq. 
(Gorgeu,  A.  ch.  (3)  61.  355.) 

Sodium  manganate,  Na2MnO4+10H2O. 

Sol.  in  H2O,  with  partial  decomp.     (Gen- 
tele,  J.  pr.  82.  58.) 

Strontium  manganate,  SrMnO4. 
Insol.  in  H2O.    (Fromherz.) 


Permanganic  acid.  . 
See  Permanganic  acid. 

Manganicyanhydric  acid,  H3Mn(CN)6. 
Not  known  in  the  free  state. 

Barium  manganicyanide,  Ba3[Mn(CN)6]2. 
Sol.  in  H2O.    (Fittig  and  Eaton.) 

Barium  potassium  manganicyanide  barium 
cyanide,    2KBaMn(CN)6,    3Ba(CN)2  + 
8H20. 
Decomp.    by   H2O.      (Lehmann,    Dissert. 

1898.) 

Calcium  manganicyanide,  Ca3[Mn(CN)6]2. 
Sol.  in  H2O.    (Fittig  and  Eaton.) 

Potassium  manganicyanide,  K3Mn(CN)6. 

Sol.  in  H2O.  (Christensen,  J.  pr.  (2)  31. 
163.) 

Sodium  manganicyanide,   Na3Mn(CN)6  + 

2H2O. 
Sol.  in  H2O.    (Fittig  and  Eaton.) 

Manganimanganic  acid. 

Barium  manganimanganate,   Ba3Mn2O8-f- 

H2O. 

Insol.  in  H2O.  Identical  with  Rosenstiehl's 
"basic  barium  manganate,"  (J.  Pharm.  1864, 
46.  344).  (Auger  and  Billy,  C.  R.  1904,  138. 
501.) 

Lithium  manganimanganate,   Li6Mn2O8+ 

H2O. 
Insol.  in  H2O.    (Auger  and  Billy.) 

Manganiperiodic  acid,  H2O,  Mn2O3,  I207. 
Wholly  insol.  in  H2O,  in  hot  dil.  or  cone. 
HNO3  and  in  hot  dil.  H2SO4.     (Price,  Am. 
Ch.  J.  1903,  30.  182.) 

Potassium  manganiperiodate,  K2O,  Mn2O3, 

I207. 

Apparently  entirely  insol.  and  unchanged 
when  boiled  with  H2O,  dil.  or  cone.  HNO3, 
or  dil.  H2SO4.  (Price.) 

Sodium    manganiperiodate,    Na2O,    Mn2O3, 

I207. 

Apparently  insol.  and  unchanged  when 
treated  with  boiling  H2O,  boiling  dil.  or  cone. 
HNO3  and  boiling  dil.  H2SO4.  (Price.) 

Manganocyanhydric  acid,  H4Mn(CN)6. 

Most  easily  decomp.  SI.  sol.  in  alcohol. 
Insol.  in  ether.  (Descamps,  A.  ch.  (5)  24. 

185.) 


486 


MANG!NOCYANIDE,  AMMONIUM  CUPROUS 


Ammonium  cuprous  manganocyanide. 

(NH4)2Cu2Mn(CN)6. 

Sol.  in  H2O;  decomp.  by  acids  and  alkalies; 
very  unstable.  (Straus,  Z.  anorg.  1895,  9. 
14.) 

Ammonium  manganous  manganocyanide, 

NH4CN,  Mn(CN),= 

(NH4)2MnMn(CN)6. 

Sol.  in  NH4CN+Aq.  (Fittig  and  Eaton, 
A.  145.  157.) 

Barium  manganocyanide,  Ba2Mn(CN)6. 
Sol.  in  cold  H2O.    (Fittig  and  Eaton.) 

Calcium  manganocyanide,  Ca2Mn(CN)6. 

Very  deliquescent.  Sol.  in  H2O;  insol.  in 
alcohol.  (Fittig  and  Eaton.) 

Cuprous  potassium  manganocyanide, 

Cu2K2Mn(CN)6. 

Sol.  in  H2O  with  si.  decomp.  Easily  de- 
comp. by  acids  and  alkalies.  (Straus,  Z. 
anorg.  1895,  9.  12.) 

Cuprous  sodium  manganocyanide, 

Cu2Na2Mn(CN)6. 

Sol.  in  H2O  with  only  si.  decomp.  Par- 
tially decomp.  by  acids.  (Straus.) 

Manganous  potassium  manganocyanide, 
KCN,  Mn(CN)2  =  K2MnMn(CN)a. 
Ppt.     Sol.  in  KCN+Aq. 

Potassium   manganocyanide,    K4Mn(CN)6  + 
3H2O. 

Very  efflorescent.  Sol.  in  H2O;  decomp.  by 
boiling. 

Potassium  manganocyanide  chloride. 

K4Mn(CN)6,  KC1. 
Easily  sol.  in  H2O.    (Descamps.) 

Sodium     manganocyanide,     Na4Mn(CN)6  + 
8H2O. 

Very  efflorescent.  Easily  sol.  in  H*O. 
(Fittig  and  Eaton.) 

Strontium  manganocyanide,  Sr2Mn(CN)6. 
As  the  Ba  comp.     (Descamps.) 

Permanganomolybdic  acid. 

See  Permanganomolybdic  acid. 

Permanganotungstic  acid. 
See  Permanganotungstic  acid. 

Manganosulphuric  acid. 
See  Sulphate,  manganic. 

Manganous  acid,  H2MnO3  =  MnO2,  H2O. 
Insol.  in  H2O.    (Franke,  J.  pr.  (2)  36.  451.) 
2MnO2,  H2O  (?).    Min.  Wad. 


Barium  manganite,  BaO,  5MnO2. 

SI.  sol.  in  HCl+Aq,  less  sol.  in  HNO3+Aq. 
(Rissler,  Bull.  Soc.  (2)  30.  111.) 

BaO,  7MnO2.    (Rousseau,  C.  R.  104.  786.) 

BaO,  2MnO2.    Insol.  in  H2O. 

BaO,  MnO2.  Insol.  in  H2O.  (Rousseau, 
C.  R.  102.  425.) 

Ba(H3Mn4Oio)2.  (Morawski  and  Stingl,  J. 
pr.  (2)  18.  92.) 

Calcium  manganite,  CaO,  5MnO2. 

Easily  sol.  in  HCl+Aq,  less  in  HNO3+Aq. 
(Rissler.) 

3CaO,  MnO2  (?).  Decomp.  by  H2O.  Sol. 
in  HCl+Aq  with  evolution  of  Cl.  Scarcely 
sol.  in  cold  HNO3,  but  sol.  on  heating.  (Du- 
fau,  A.  ch.  1897,  (7)  12.275.) 

2CaO,  MnO2.  Sol.  in  dil.  min.  acids. 
(Rousseau,  C.  R.  116.  1060.) 

CaO,  2MnO2.    (Rousseau,  C.  R.  102.  425.) 

CaO,  3MnO,. 

CaO,  MnO2.  Sol.  in  fuming  HCl+Aq,  but 
not  in  dil.  HNO3+Aq.  (Rousseau,  C.  R.  116. 
1060.) 

Chromium     manganite,     Cr2O3,     3MnO2  = 

Cr2(MnO3)3. 

Slowly  decomp.  by  acids.  (Groger,  Z. 
anorg.  1905,  44.  458.)  • 

Cobaltous  manganite,  CoO,  MnO2+2H2O. 
Ppt.  (Salinger,  Z.  anorg.  1903,  33.  352.) 
+4H2O.  Ppt.  (Salinger.) 

Cobalt  copper  manganite,  CoO,  CuO,  2MnO2 

+4H2O. 

Min.  Asbolite.  Sol.  in  HCl+Aq,  with 
evolution  of  Cl. 

Cupric  manganite,  CuO,  4MnO2. 

(Gorgeu,  Bull.  Soc.  1903,  (3)  29.  1167.) 
CuO,  8MnO2+3H2O.     (Baubigny,  C.  R. 

1897,  124.  955.) 

Cupric  manganous  manganite,  4CuO,  MnO, 
7MnO2+8H2O. 

Ppt.    (Salinger,  Dissert.  1902.) 

Mn2O3,  3CuO.  Sol.  in  HCl+Aq.  (Schnei- 
der, Am.  Ch.  J.  9.  269.) 

Lead  manganite,  PbO,  5MnO2. 

Not  attacked  by  cone,  acids;  sol.  in  aqua 
regia.  (Rissler.) 

Magnesium  manganite,  2MgO,  MnO2. 
(Lemoine,  Ann.  Min.  (7)  3.  5.) 
+zH2O.    (Vollard.) 


Manganous   manganite,   Mn3Os 
2MnO2. 

(Reissig,  A.  103.  27.) 

Mn6On=MnO,    5MnO2.      (Veley,    Chem. 
Soc.  38.  581.) 


MERCURIAMMONIUM  NITRATE 


487 


3MnO2j  2MnO.  Decomp.  by  dil.  H2SO4-h 
Aq.  (Franke,  J.  pr.  (2)  36.  166.) 

3MnO2,  MnO+H2O.    Min.  Varvicite. 

Manganous    zinc    manganite,    MnO,    ZnO, 

MnO2. 

(Gorgeu,  Bull.  Soc.  1903,  (3)  29.  1168.) 
2MnO,  ZnO,  2MnO2.    (Gorgeu.) 

Potassium  manganite,  K2O,  2MnO2. 

Insol.  in  H2O. 

KoO,  5MnO2. 

K2O,  7MnO2+3H2O. 

K2O,  8MnO2+3H2O  =  KH3Mn4O10.  (Mor- 
awski  and  Stingl,  J.  pr.  (2)  18.  91.) 

Does  not  exist.  (Wright  and  Menke. 
Chem.  Soc.  37.  22.) 

K2O,  10MnO2. 

K2O,  16MnO2+6H2O.  Sol.  in  cone.  HC1+ 
Aq.  (Rousseau,  C.  R.  114.  72.) 

Silver  manganite,  AgH3Mn4Oio. 

(Morawski  and  Stingl,  J.  pr.  (2)  18.  92.) 
Ag2MnO3.    Ppt.    (Gorgeu,  C.  R.  110.  958.) 

Silver  (argentous)  manganite,  Ag4O, 

Mn2O3  (?). 

Insol.  in  cold  dil.  HNO3+Aq,  and  separ- 
ates Mn2O3  on  warming.  Insol.  in  NH4OH  + 
Aq.  (Rose,  Pogg.  101.  229.) 

Silver    (argentoargentic)    manganite,    Ag4O, 

2Ag2O,  Mn2O3  (?). 
(Rose.) 

Sodium  manganite,  Na2O,  5MnO2. 

Insol.  in  H2O.    (Rousseau,  C.  R.  103.  261.) 
Na2O,   12MnO2.     Insol.  in  H2O.     (Rous- 
seau.) 

+4H2O.    (Rousseau,  C.  R.  112.  525.) 
Na2O,  8MnO2+5H2O.    (Rousseau.) 
Na2O,  16MnO2+8H2O.    (Rousseau.) 

Strontium  manganite,  MnO2,  SrO. 

Insol.  in  H2O. 

2MnO2,  SrO.  Insol.  in  H2O.  (Rousseau, 
C.  R.  101.  167.) 

MnO2,  5SrO.  Sol.  in  HC1,  or  HNO3+Aq. 
(Rissler,  Bull.  Soc.  (2)  30.  110.) 

Zinc  manganite,  ZnO,  5MnO2. 

Insol.  in  H2O.    (Rissler.) 

ZnO,  4MnO2.  (Gorgeu,  Bull.  Soc.  1903, 
(3)  29.  1168.) 

3ZnO,  MnO2+7^H20.  (Salinger,  Dissert. 
1902.) 

27ZnO,  2MnO2+25H2O.  Insol.  in  H2O. 
(Salinger.) 

Manganyl  chloride,  MnO3Cl. 
Decomp.  by  H2O.    (Aschoff,  J.  pr.  81.  29.)  ' 


Melanocobaltic  chloride, 

Co2(NH3)6Cl4NHoCl,  or 

Co2(NH3)6Ci5NH2. 

Very  si.  sol.  in  cold  H2O  or  very  dil.  HCl-f 
Aq.  Decomp.  by  long  standing  or  warming. 
Cold  cone.  HC1  or  dil.  H2SO4+Aq  does  not 
attack,  but  decamp,  on  warming.  HNO3-h 
Aq  decomp.  on  warming.  Sol.  in  cold  H2SO4 
or  NH4OH+Aq;  from  both  solutions  it  can 
be  precipitated  by  HCl+Aq.  (Vortmann,  B. 
10.  1455.) 

chloroplatinate,  Co2(NH3)6NH2Cl5, 

PtCl4. 

Ppt.    (Vortmann,  B.  16.  1902.) 
Co2(NH3)6NH2Cl3(OH)2,     PtCl4.       Ppt. 

(Vortmann.) 

mercuric  chloride, 

Co2(NH3)6(NH2)Cl3(OH)2,  3HgCl2+ 

H2O. 

Ppt.  Difficultly  sol.  in  cold  H2O,  quite 
easily  in  warm  H2O  acidified  with  HC1. 
(Vortmann.) 

chloride  chromate, 

Co2(NH3)cNH2Cl3Cr207  +H2O. 
Sol.  in  hot  H2O.    (Vortmann.) 

Mercurammonium  comps. 
See  Mercury  ammonium  comps. 

Mercuriammonium  bromide,  Hg(NH2)Br. 
See  Dunercuriammonium  ammonium  bro- 
mide. 

Mercuriammonium  chloride,  Hg(NH2)Cl. 

See  Z)?'mercuriammoniuni  ammonium  chlo- 
ride. 

Mercuriammonium  oxy^mercuriammonium 
chloride,  4Hg(NH2)Cl,  NH2(HgOHg)Cl. 

(MiUon.) 

Correct  composition  is  D?'mercuriammon- 
ium  ammonium  chloride,  NHg2Cl?  NH4C1, 
which  see.  (Balestra,  Gazz.  ch.  it.  21,  2. 
294.) 

Hg(NH2)Cl,  2NH2(HgOHg)Cl.     (Mfflon.) 

Correct  composition  is  Drmercuriammon- 
ium  mercuric  chloride,  2NHg2Cl,  HgCl2  + 
H2O,  or  Zh'mercuriammonium  hydrogen  chlor- 
ide, NHg2Cl,  HC1.  (Balestra.) 

Mercuriammonium  nitrate,  2NH3,  2HgO, 
N2O6  =  NH2HgNO3 + ^H2O. 

Easily  decomp.  by  HC1,  or  alkali  sul- 
phides+Aq.  SI.  sol.  in  HNO+Aq.  Insol. 
in  H2SO4,  NH4OH,  or  KOH+Aq.  (Mits- 
cherlich.) 

Is  cfo'mercuriammonium  ammonium  ni- 
trate, NHg2NO3,  NH4NO3+H2O.  (Pesci, 
Gazz.  ch.  it.  20.  485.) 


MERdJKIAMMOff JUM  OXYMEBCCIttAMMOXIUM  NITRATE 


Decomp.  by  boiKng  with  H2O,  which,  dis- 
solves out  XHfNOj,    Sol.  in  XH^XO^HhAq 


containing   .VH/)H.       Mitscherlieh.) 

Is    '/imercuriammoniiim     ammonium    ni- 


Gazz,  ch,  it,  20*  485,) 

Mercuriammonium    oxyr/?,meTCurianimonittni 
ttdphate.    (NHjHg)»SO4, 

2CRHfcaH*),0o* 

Boiling  H^  dissolves  oat  H^SO*  Gradu- 
ally decomp.  by  boiling  KOH+Aq.  Com- 
pletely sol.  in  NH<CH-Aq.  Sol.  in  cone,  or 
dil,  HCl,  or  rery  dil.  H2SO4-f-Aq.  Insol.  in 
cone,  or  dil.  H.VOa+Aq  or  cone.  H2SO4. 
(Schneider.) 

Correct  formula  is  7(NHg2)2SO4f  (NH4)2SO4 
-fl2H;tO,  r/?;mercuriammonium  ammonium 
Bulphate,  (Pesci,  Gazz.  ch.  it.  20.  485.) 

Mercuric  ammonium     chloride    (fusible 

white  precipitate),  Hg(NH3)2Cl2. 
I«  <&'mercuriammonium  ammonium  chlo- 
ride, Hg2NCl,  3NH4C1,  which  see.    (Ram- 
melsberg J.  pr.  38.  558.) 

Mercuric/ammonium  mercuric  chloride, 
Hg(XH,)2Cl2,  HgCl2. 

Insol.  in  f[2O,  but  gradually  decomp.  by 
boiling  therewith.  fRose,  Pogg.  20.  158.) 

Partly  sol.  in  H2O.     fKane.) 

Mercuri'/?;ammonium  iodide,  Hg(NH3)2I2. 

H2O  extracts  all  the  NH?.  Partly  sol.  in 
little  alcohol.  Partly  sol.  in  ether  without 
decomp.  (Nessler.) 

Correct  composition  is  fifc'mercuriammon- 
ium  ammonium  iodide,  NHg2I,  3NH4I. 
(Pesci,  Gazz.  ch.  it.  20.  485.) 

Mercuri'/iammonium   cupric   iodide,   4NH3, 
CuI2,  HgI2. 

Decomp.  by  H2O.     Sol.  in  alcohol -f 
HC7H8O2.     (Jorgensen,  J.  pr.  (2)  2.  347.) 

2Hg(NH,)jI,,  CuI2.  (Decomp.  by  H2O. 
(Jorgensen.) 

Mercuric/ammonium  iodide,  Hg(NH3)2I2. 

Decomp.  by  H2O.  Partly  sol.  in  a  little 
alcohol.  Partly  sol.  in  ether.  (Nessler.) 

Correct  composition  is  efamercuriammon- 
ium  ammonium  iodide,  NHg2I,  3NHJ. 
(Pesci.) 

Mercuridiammonium    mercuric    iodide, 
Hg(NH,),,  HgI2,  or  NH3,  HgI2. 

Decomp.  by  H2O  or  dil.  acids.  (Caillot 
and  Cornol,  J.  Pharm.  9.  381.) 

Correct  composition  is  r/rmercuriammon- 
iuin  ammonium  momirir.  iodide,  UNTHgJ, 
8NHJ,  4HgI2.  (Pesci,  Gazz.  ch.  it.  20. 


Mercuri^ammonium  sulphate 

Decomp.  with  H/X 

Does  not  exist.  (Peao,  Gan.  A.  it,  JO. 
«K 

-HH2O,  Decomp.  by  HjO.  Eawly-  aoL  in 
HC3,  very  dfl.  HaSC^-f-Aq,  or  HXO»-|rAq. 
Insol.  in  cone.  HXO3  -j-Aq.  SoL  in  (XH^yBO* 
+Aq  or  NH4Cl-f-Aq.  Decomp.  by  KOH-(- 
Aq,  (Schneider,  J.  pr.  75. 136.) 

Correct     composition    is 

ammonium  sulphate'    (Pesci.) 
/^'mercuriammonium  acetate, 


Insol.  in  HjO  or  alcohol.  Sol.  in  HCl  or 
XH4C2H3Oz-hAq.  (Balestra,  Gazz.  ch.  it. 
22,2.563.) 

ZKmercuriammonium     ammonium     acetate, 

XHg2C2H302,    3XH4C2H302+H20. 
Deh'quescent;  sol.  m  a  little  H2O  without 
decomp.,  but  decomp.  into  XHg2C2H3O2  and 
NH^sH^*  by  excess  of  HjO.     (Balestra.) 

arsenate,  XHgjH2AsO4. 

(Hirzel,  Zeit.  Pharm.  1863.  3.) 

bromate,  XHg2BrO3-|-l^HjO. 

Ppt.    (Rammelsberg,  Pogg.  56.  82.) 
Is   oxyrfimercuriammonium    bromate, 

(NH2Hg20)Br03. 

bromide,  NHg2Br. 

Insol.  in  H2O  or  HNO3.  Sol.  in  HCl-f-Aq. 
(Pesci,  Gazz.  ch.  it.  19.  509.) 

Sol.  in  KI,  or  Na2S2O3+Aq  with  evolution 
of  NH3.  (Balestra,  Gazz.  ch.  it.  22,  2.  558.) 

Sol.  in  ammoniacal  solutions  of  ammonium 
salts  and  in  aq.  .acids.  (Franklin.  J.  Am 
Chem.  Soc.  1905,  27.  839.) 

—  ammonium  bromide,  XHg2Br,  XH4Br. 

Decomp.  by  H2O.  (Pesci,  Gazz.  ch.  it.  19. 
511.) 

4NHg2Br,  5N54Br.  Decomp.  by  H2O. 
Insol.  in  (NH4)2CO3+Aq.  Sol.  in  cone,  or 
dil.  HCl 4- Aq.  Insol.  in  HNO3+Aq.  (Pesci.) 

NHg2Br,  3NH4Br.  Decomp.  by  H2O. 
Easily  sol.  in  HCl+Aq.  Insol.  in  alcohol. 
(Pesci.) 

Sol.  in  NH4Br,  NH4C1,  or  NHJ+Aq; 
sol.  in  KI,  or  Na2S203+Aq. 

—  mercuric  bromide,  2XHg2Br,  HgBr2. 
Ppt.     Sol.  in  HBr  and  in  HCl.     (Ray, 

Chem.  Soc.  1902,  81.  649.) 

—  carbonate,   (NHg2)2CO3+2H2O. 

Ppt.  Not  decomp.  by  KOH+Aq,  but 
easily  by  K2S,  or  KI+Aq.  (Rammelsberg, 
J.  pr.  (2)  38.  567.) 


MEBCTRIAMMOXIOi  AMMONIUM  NITRATE 


by  eon  OIL  a&jM^f-jujg 
sfiivcd  thereby, 

^LKL. 

0aL  m  l&JL  o 
,:    VH; 

-HjO.    Xearfy  iMoL  in  H/>; 
in  HXQ*  aad  Hd-f-Aq.    Xot 
KOHHrAq.    Drccnp.  by  KO,  X 
Aq.    (ffiMiiMniA,FqBB-4aLl&Lj> 


-A: 


soL 
by 


2HCL 

Conceit  ftwmpiMftioii  of  mereim 
snide  chloride.     fTBaksfra,  Gazz.  eh.  it  M, 

*S?L. 

Decamp,  by  B^O. 

XHsiCL  HCL     Decomp.  by  HdO.      Ba- 
--,    .    : 

fflOL   SoLinHdO.    (Ray,Froe. 


by  HaO,  n»dflj  by  KOH+Aq. 
A.  eh.  1911r  (8)  tt.  212L) 
Fpt.     SoL  in  HBr.     f  Biy,  Ftoe. 
Soe.  1902,  1BL 


ofwhathasbeenealled 
B«m- 

Inaol.VeoH'SttHnp.  by  hot  H4)  (M3^ 
n,  A.  eh.  (3)  18.  413.)  SoL  in  GOO  pta. 
HjO.  (Wittrtein.)  SoL  in  719.98  pts. 
H^OatlS.75".  (AbL)  InsoL  in  aleohoL 

SoL  in  acids,  even  in  HCJBdOx+Aq,  abo 
in  XH^XO^  (X^)j^O^,  and 
Aq.    (Pekmze  and  Fremy.) 

Oto*t)m 

SI  soL  in  alkali  ehlorides+Aq,  which  par- 
tially decamp.  Miahle,  A.  eh.  (3)  6.  180.) 

Decomp.  by  KOH-f  Aq.  SoL  in  KI,  or 
NaAO,+Aq,  with  evolution  of  XH^  (Ba- 
lesbn.) 

When  freshly  prepared  is  soL  in  o 
XH/JH-rAq.      (Saha   and   Choudhuri, 

1910,  67.  359.) 

in  excess  of  <XH4)^PO4+Aq. 

-  of  Xa*HP04+Aq-    (Carnegie  and 

Burt,  C.  N.  1897, 7«.  175.) 

InsoL  in  excess  of  XH«OH+Aq.  (Car- 
negie and  Bart.) 

XHgjd,  3XH4C1  (Fusible  white  precipi- 

tate  . 

Correct  composition  of  what  has  been 
called  mercurid  ammonium  chloride, 
Hg  XH^^CU.  (Rammelsberg,  J.  pr.  (2) 
38. 558.) 

Decomp.  by  hot  H/).  SoL  in  acids,  even 
HCjHjOi-hAq.  Not  deeomp.  by  cold,  but 
by  bofling  KOH-f  Aq.  (WeyL) 

SoL  in  warm,  less  in  cold  NH^H-f  Aq. 
(Mitscheriich.) 

SoL  in  KI,  or  Xa&O*+Aq,  with  evolution 
ofXH,.  (Balestra.) 

Sol.  in  10%  HNOa,  H^SO4  and  acetic 
acid.  CHofmann  and  Marburg,  A.  1899, 
305.  19S. 


HO  or  HXOsHhAq. 


2XH4O^ 

InsoL  in  HXO^.  (Bammefaberg,  J.  pr.  (2) 
38.568.) 

iodide,  XHg*L 

InsoL  in  Hrf).  SoL  in  Hd-f  Aq.  De- 
camp, by  boning  with  KOH+Aq  or  KO+ 
Aq.  (Weyl,  Pogg.  12L  601.)  Deeomp. 
bybotKl,orNaAO,+Aq.  (Bafcslra.) 

Decomp.  by  dflute  HCL  Sol.  in  ammon- 
salts-f  Aq.  (Franklin.  Z.  anorg.  1905, 


,  NHgJ,  3NHJ. 
of  mercuri'/iammon- 
.    (Peso,  Gazx.  ch.  H. 


Correct 
miodkfe, 

s. 


SXHgJ,  8NHJ,  4HgI,.    Correct  formula 
for    mercuri^iammonium    mercuric    iodide, 
Hgl,.    (PescL) 


nitrate, 


InsoL  in  H,O.  (Bammdsberg,  J.  pr.  (2) 
38.  566.) 

SoL  in  KI,  or  XaAOj-f-Aq,  with  evolution 
ofXH*  (Balestra,  Gaxx.ch.it.  M,  2.  560.) 

+H/>.  (Hofmann  and  Marburg,  A.  1899, 
905.  212.) 

SL  soL  in  HXO,.  (Bay,  Z.  anorg.  1902, 
33.209.) 


—  —  ammonium  nitrate,  NHgjNOj, 
+H,0. 

Correct  formula  for  mercuriammonium 
nitrate,  XHjHgXOj-h^iHjO.  (Pesci,  Gaxx. 
ch.  it.  20.  485.) 

XHg2XO,,  2NH4NO,+2HsO.    Correct  for- 


490 


MERCURIAMMONIUM  NITRITE 


mula  for  oxy^'mercuriammonium  ammonium 
nitrate,  (NHg2OH2)NO3,  2NH4NO3+H2O. 
(Pesci.) 

NHg2N03,  3NH4N03.  Decomp.  by  cold 
H2O;  sol.  in  NH4OH+Aq.  (Pesci.) 

3NHg2NO3,  NH4NO3+2H2O.  Correct  for- 
mula for  mercuriammonium  oxyrftmercuriam- 
monium  nitrate,  NH2HgNO3,  (NHg2OH2)NO8 
+H2O.  (Pesci.) 

Di'mercuriammonium  nitrite,  NHg2NO2. 

Readily  sol.  in  warm  HC1  or  HBr.  (Ray, 
Chem.  Soc.  1902,  81.  648.) 

+  3/£H2O.  Ppt.  SoLinHCl.  (Ray,  Proc. 
Chem.  Soc.  1902,  18.  85.) 

+H2O.  (Hofmann  and  Marburg,  A.  1899, 
305.214.) 


oxide,  (NHg2)20. 


Slowly  decomp.  by  H2O.  Sol.  in  HC1,  or 
HNO3+Aq.  Decomp.  by  hot  KOH,  or  KC1 
+Aq.  (Weyl,  Pogg.  121.  601.) 

Sol.  in  KCN+Aq  by  heating  4-5  hours 
at  130°.  Not  completely  sol.  in  HC1  owing 
to  formation  of  Hg2Cl2.  (Gaudechon,  C.  R. 
1907,  144.  1419.) 

phosphate,   (NHg2)2PO4,   2NHg2OH  + 

10H20. 

(Rammelsberg,  J.  pr.  (2)  38.  567.) 
Sec  Oxycfo'mercuriammonium  phosphate. 

ammonium  salicylate, 

2NHg2C6H4OHCO2,  5NH4C6H4OHCO2. 
Decomp.  by  H2O.     Sol.  in  NH4C2H3O2, 
HC1,  or  KI+Aq.    (Balestra.) 

selenate,  (NHg)2SeO4+2H2O. 

Ppt.  Insol.  in  H2O;  sol.  in  NH4OH+Aq. 
(Cameron  and  Davy,  C.  N.  44.  63.) 

sulphate,  (NHg2)2SO4+2H2O. 

Insol.  in  H2O.  Easily  sol.  in  HCl+Aq. 
(Rammelsberg,  J.  pr.  (2)  38.  565.)  Sol. 
(Kane),  insol.  (Hirzel)  in  HNO3+Aq. 

Sol.  in  KI,  or  Na2S2O3+Aq  with  evolution 
of  NH3.  (Balestra.) 

+H2O.  Insol.  in  H2O;  sol.  in  HC1.  (Ray, 
Chem.  Soc.  1905,  87.  9.) 

ammonium  sulphate,  (NHg2)2SO4, 

3(NH4)2SO4+4H2O. 

Correct  formula  for  mercuriffo'ammonium 
sulphate,  2NH3,  HgO,  SO3+H2O.  (Pesci, 
Gazz.  ch.  it.  20.  485.) 

5(NHg2)2SO4,     14(NH4)2SO4+16H2O. 
(Pesci.) 

7(NHg2)2S04,  (NH4)2S04  +  12H20.  Cor- 
rect formula  for  mercuriammonium  oxycfo'mer- 
curiammonium  sulphate,  (NHg2H2)2SO4, 
3(NHg2OH2)2SO4.  (Pesci.) 


Dimercuriannnonium  tartrate, 
(NHg2)2C4H406+2^H20. 
Insol.  in  H2O.    Sol.  in  HC1,  KI,  Na2S2O3, 
NH4C2H3O2,  or  (NH4)2C4H4O6+Aq.     (Bal- 
estra, Gazz.  ch.  it.  22,  2.  563.) 

ammonium  tartrate,  2(NHg2)2C4H4O6, 

(NH4)2C4H406+H20. 
As  above.    (B.) 

Tnmercuriammonium  sulphate, 

(NHg2)(NHgH2)S04+2H20. 
Decomp.  by  H2O.    (Millon.) 
Does  not  exist.     (Pesci,  Gazz.  ch.  it.  20. 

485.) 

Dimercuriarsonium  mercuric  chloride, 

AsHg3Cl3=AsHg2Cl,  HgCl2. 
Decomp.    by   H2O.      Decomp.    by   warm 
HNOs+Aq.    (Rose,  Pogg.  51.  423.) 

Mercurimidosulphonic  acid, 

(H03S)4N2Hg. 
Very  unstable.    (Berglund,  B.  9.  256.) 

Barium  mercurimidosulphonate, 

Ba2(S03)4N2Hg+5H20. 
(Berglund,  B.  9.  256.) 

Cadmium ,  Cd2HgN2(SO3)4+12H2O. 

Unstable;  si.  sol.  in  H2O.    (Berglund,  Bull. 
Soc.  (2)  25.  452.) 

Cobalt ,  Co2HgN2(SO3)4+15H2O. 

Sol.  inH2O.    (B.) 

Copper ,  Cu2HgN2(SO3)4  +  15H2O. 

Very  sol.  in  H2O.    (B.) 

Magnesium ,  Mg2HgN2(SO3)4+15H2O. 

Very  sol.  in  H2O.    (B.) 

Manganous ,  Mn2HgN2(SO3)4+10B[2O. 

Unstable.    (B.) 

Mercuric ,  (Hg2O)2HgN2(SO3)4. 

Nearly  insol.  in  H2O.    (B.) 


Nickel 

(B.) 


-,  Ni2HgN2(S03)4  +  15H20. 


Potassium ,  (KO3S)4N2Hg+4H2O. 

Precipitate.    (Raschig,  A.  241.  161.) 

-,  (AgS03)2(KS03)2HgN. 


Potassium  silver 

+3H2O. 
SI.  sol.  in  H2O.    (Berglund.) 

Sodium ,  (NaSO3)4HgN2+5H2O. 

More  sol.  in  H2O  than  K  salt.    (Berglund.) 

Strontium ,  Sr2(SO3)4HgN2+15H2O. 

More  sol.  than  Ba  salt.    (B.) 


MERCURY 


491 


Zinc  mercurimidosulphonate, 

Zn2(SO3)4HgN2  +  15H2O. 
Very  sol.  in  H2O.    (B.) 

£imercuriphosphonium    mercuric    bro- 
mide, 2PHg2Br,  HgBr2. 
(Lemoult,  C.  R.  1907,  146.  1176.) 

Zh'mercuriphosphonium    mercuric    chloride, 

HgCl2,  PHg2Cl. 

(Lemoult,  C.  R.  1907,  145.  1176.) 
+1^H2O.     Decomp.  by  hot,  slowly  by 

cold  H2O  into  Hg,  HC1,  and  H3PO3.    Decomp. 

by  acids  or  alkalies.    (Rose,  Pogg.  40.  75.) 

Dmiercuriphosphonium  mercuric  iodide, 

HgI2,  PHg,I. 

Slowly  decomp.  by  cold  or  warm  H2O, 
quickly  by  MOH+Aq  .  Not  attacked  by 
HC1  or  H2SO4+Aq.  Rapidly  attacked  by 
HNO3  and  aqua  regia.  (Lemoult,  C.  R. 
1904,  139.  479.) 

Zh'mercuriphosphonium     mercuric     nitrate, 
P2Hg3,       6HgO,       3N206  =  2[PHg2N03, 
Hg(NO,U  3HgO. 
(Rose,  Pogg.  40.  75.) 

Dimercuriphosphonium    mercuric    sulphate, 
P2Hg3, 6HgO,  4S03+4H20  =  (PHg2)2SO4, 
3HgS04,  2HgO+4H20. 
Sol.  in  aqua  regia.    (Rose,  Pogg.  40.  75.) 

Mercuric  acid. 

Calcium  mercurate  (?). 
(Berthollet,  A.  ch.  1.  61.) 

Potassium  mercurate,  K2O,  2HgO. 

Gradually  decomp.  by  H2O;  less  rapidly  by 
absolute  alcohol.  (St.  Meunier,  C.  R.  60. 

557.) 

Sodium  mercurate,  Na2O,  HgO. 
(Bettekoff,  Bull.  Soc.  (2)  34.  328.) 

Mercuroammonium  chloride, 

Hg(NH3)Cl. 
(Rose,  Pogg.  20.  158.) 
Mixture  of  Hg,   HgNH2Cl,   and   NH4C1. 
(Barfoed,  J.  pr.  (2)  39.  201.) 

nitrate,  (NHg2Ha)NO3,   "Hahnemann's 

soluble  mercury." 

Sol.  in  hot  HC1,  and  HC2H3O2+Aq.  De- 
comp. by  NH4OH+Aq,  or  NH4  salts +Aq. 
Probably  mixture  of  mercurous  salts  and  Hg. 

Mercurodiammonium  chloride, 

Hg2(NH3)2Cl2. 

Easily  decomp.    (Rose,  Pogg.  20. 158.) 
Mixture  of  Hg,   NH2HgCl,   and   NH4C1. 
(Barfoed,  J.  pr.  (2)  39.  201.) 


Mercurod; 'ammonium  fluoride, 

Hg2(NH3)2F2  (?). 
Decomp-.  by  H2O.     (Finkener,  Pogg.  110. 

147.) 

Mercurosulphonic  acid. 

Mercurosulphonates,  Hg(SO3M)2. 

Correct  composition  for  the  double  sul- 
phites, HgSO3,  M2SO3.  (Divers  and  Shimid- 
zu,  Chem.  Soc.  49.  583;  Earth,  Z.  phys.  Ch. 
9.  195.) 

Mercuroxy-comps. 
See  Oxymercur-  comps. 

Mercury,  Hg. 

Not  attacked  by'H2O.  Not  attacked  by 
boiling  cone.  HC1  or  dil.  H2SO4+Aq.  Easily 
sol.  in  dil.  or  cone.  HNO3+Aq:  also  in  HBr 
orHI+Aq. 

Not  attacked  by  pure  HNO3  unless  heated, 
but  readily  attacked  by  cold  dil.  HNO3+Aq 
containing  NO.  (Millon.) 

Anhydrous  H2SO4  attacks  Hg  gradually 
at  ord.  temp.  (Berthelot,  C.  R.  1897,  126. 
749.) 

H2S04  attacks  only  when  hot  and  cone. 
(Ditte,  A.  ch.  1890,  (6)  19.  68.) 

Cone.  H2SO4  does  not  attack  dry  or  moist 
Hg  either  with  or  without  air.  (Pitman,  J. 
Am.  Chem.  Soc.  1898,  20.  100.) 

H2SO4  attacks  Hg  at  20°  if  it  contains 
99.7%;  does  not  attack  if  it  contains  only 
95.6%.  (Baskerville,  J.  Am.  Chem.  Soc. 
1898,  20.  515.) 

Insol.  in  H2SO3+Aq  alone  or  in  presence 
of  HC1  or  dil.  H2SO4.  (Berthelot,  A.  ch. 
1898,  (7)  14.  198.) 

Not  attacked  by  HF+Aq  at  any  temp. 
(Gay-Lussac.) 

HI  dissolves  Hg  rapidly  at  ord.  temp. 
(Norris  and  Cottrell,  Am.  Ch.  J.  1896,  18. 
99.) 

More  rapidly  attacked  by  HBr+Aq  than 
by  HCl+Aq.  Rapidly  acted  upon  by  HI  in 
absence  of  O.  (Bailey,  Chem.  Soc.  1888,  53. 
760.) 

Not  attacked  by  pure  HCl+Aq,  but  in 
presence  of  O,  Hg2OCl2+H2O  is  formed. 
Action  is  apparently  less  in  sunlight  than  in 
the  dark.  (Bailey,  Chem.  Soc.  1888,  53.  759.) 

Small  amts.  of  ferric  salts  hinder  action 
of  HNOs  on  Hg,  but  it  is  hastened  bv  pres- 
ence of  Mn(NO3)2  or  NaNO^.  (Ray/Chem. 
Soc.  1911,  99.  1015.) 

HNO3  under  33%  does  not  attack  Hg  if 
metal  and  acid  are  kept  in  motion  and  HNO2 
is  absent.  (Veley,  B.  1895,  28.  928.) 

Rapidly  sol.  in  HC1O.  (Balard,  Dissert. 
1834.) 

Alkali   chlorides +Aq   in   presence   of   air 
decomp.  Hg;  action  is  not  increased  by  heat. 
Miahle.) 

Insol.  in  alkali  chlorides +Aq  in  neutral  or 


492 


MERCUROUS  ACETYLIDE 


alkaline  solution.     (Bhaduri,  Z.  anorg.  1897. 
13.  407.) 

Very  sol.  in  cone,  solution  of  I  in  KI+Aq. 
(Varet,  Bull.  Soc.  1897,  (3)  17.  451.) 

Slowly  sol.  in  KC1  or  KI+Aq  in  presence 
of  air.  (Palmaer,  Z.  phys.  Ch.  1907,  59.  136.) 

Slowly  sol.  in  Na2S+Aq  in  presence  of  air. 
(Palmaer,  Z.  phys.  Ch.  1907,  59.  137.) 

Hg  is  appreciably  sol.  in  the  sulpho  salts  of 
Mo,  W,  V,  As,  Sb  and  Sn.  (Storch,  B.  1883, 
16.  2015.) 

Persulphates  in  alkali  or  neutral  solution 
attack  Hg.  (NH«)&Oi  in  NH4OH  solution 
has  strongest  action.  This  dissolves  Hg  by 
repeated  shaking  at  high  temp.  (Tarugi, 
Gazz.  ch.  it.  1903,  33,  (1)  127.) 

Insol.  in  KCN+Aq.'  (Elmer,  J.  pr.  1888, 
(2)37.442.) 

Slowly  sol.  in  KCN+Aq  in  presence  of  air. 
(Palmaer,  Z.  phys.  Ch.  1907,  59.  136.) 

Sol.  in  considerable  quantity  in  6%  KCN  + 
Aq.  (Goyder,  C.  N.  1894,  69.  268.) 

Most  sol.  in  K4Fe(CN)6+Aq  when  KOH 
is  present.  (Smith,  J.  Am.  Chem.  Soc.  1905, 
27.  544.) 

Hg  dissolves  in  Br2  in  the  presence  of  KBr 
si.  faster  than  in  I2  but  in  CuBr2  much  more 
slowly.  (Van  Name  and  Edgar,  Am.  J.  Sci. 
1910,  (4)  29.  255.) 

Not  attacked  by  PC13  even  at  350°. 
(Moissan,  A.  ch.  1885  (6)  6.  457.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  829.) 

%  ccm.  oleic  acid  dissolves  0.0075  g.  Hg 
in  6  days.  (Gates,  J.  phys.  Chem.  1911,  15. 
143.) 

Mercurous  acetylide,  Hg2C2  +H2O. 

(Burkard  and  Travers,  Chem.  Soc.  1902 
81.  1271.) 

Mercuric  acetylide,  basic,  2HgO,  3HgC2  + 

2H20. 

(Burkard  and  Travers,  Chem.  Soc.  1902 
81.  1272.) 

Mercuric  acetylide,  HgC2. 

Very  sol.  in  HC1  with  evolution  of  H2C2 
(Keiser,  Am.  Ch.  J.  1893,  15.  535.) 

+  VsH2O.  Insol.  in  H2O,  alcohol  and  ether 
Sol.  in  NH4  acetate +Aq,  and  in  KCN+Aq 
SI.  attacked  by  cold  HC1,  easily  by  hot 
Easily  sol.  in  HNO3.  Dil.  H2SO4  attacks 
slowly;  cone,  causes  explosion.  (Plimpton 
and  Travers,  Chem.  Soc.  1894,  65.  267.) 

Mercuric  acetylide  chloride,  HgC2,  HgCl5 


Not  acted  upon  by  dil.  HC1.  Decomp.  bj 
fuming  HNO3  or  aqua  regia.  Insol.  in  al 
cohol  and  ether.  (Keiser,  Am.  Ch.  J.  1893 
15.  538.) 

Mercuric  acetylide  mercuromercuric  chloride 

HgC2,  HgCl,  HgCl2+H20. 
Insol.  in  all  ordinary  solvents.     (Biltz  an 
Mumm,  B.  1904,  37.  4420.) 


Mercurous  amidofluoride,  HgNH2F. 
Insol.  in  H2O,  HNO3  and  H2SO4.    Sol.  in 
il.  HC1. 

Probably  cfo'mercuriammonium  ammonium 
luoride,  NHg2F,  NH4F.  (Bohm,  Z.  anorg. 
904,43.327.) 

Mercury  ammonium  comps. 


Mercuroammonium  comps.,  NH3HgR. 
Dimercuroammonium  comps.,  NH2Hg2R. 
Mercurous  chloramide,  Hg(NH2)Cl. 
Dimercuriammonium  comps.,  NHgR. 

Mercuric  chlor-,  brom-,  etc.,  amide, 
Hg(NH2)R. 

MercurWiammonium  comps.,  Hg(NH3)2R. 
Mercuriammonium  comps.,  HgNH2R. 
Diinercuricframmonium  comps.,  Hg2N2H4R. 
TVimercuriammonium  comps.,  N2H2Hg3R. 

Oxy^Tmercuriammonium.  comps., 
NH2Hg2O)R. 

Mercurous  arsinchloride,  AsHgCl. 

Decomp.  by  H2O.  (Capitaine,  J.  Pharm. 
25.  559.) 

Mercurous  arsinchloride  chloride,  AsHg2Cl2 

=  2AsHgCl,  Hg2Cl2  (?). 
Decomp.  by  H2O.    (Capitaine.) 

Mercurous  azoimide,  HgN3. 

Wholly  insol.  in  H2O.  (Curtius,  B.  24. 
3324.) 

1  1.  H2O  dissolves  0.25  g.  (Wohler  and 
Krupko,  B.  1913,  46.  2050.) 

Mercuric  azoimide,  HgN6. 

Sol.  in  H2O  especially  when  hot.  (Ber- 
thelot  and  Vieille,  Bull.  Soc.  1894,  (3)  11. 
747.) 

Moderately  sol.  in  H2O.  (Wohler  and 
Krupko,  B.  1913,  46.  2050.) 

Mercuric  bromamide,  Hg(NH2)Br. 

Insol.  in  H2O  and  alcohol.  SI.  sol.  in 
NH4OH+Aq.  (Mitscherlich,  J.  pr.  19.  455.) 

Correct  composition  is  dimercuriammon- 
ium  ammonium  bromide,  Hg2NBr,  NH4Br, 
which  see.  (Pesci,  Gazz.  ch.  it.  19.  511.) 

Mercurous  bromide,  Hg2Br2. 

Solubility  in  H2O=9.1XlO-7  g.  equiv. 
per  1.  (Bodlander,  Z.  phys.  Ch.  1898,  27.  61.) 

Solubility  in  H2O=7XlO^  mols.  per 
liter  at  25°.  (Sherrill,  Z.  phys.  Ch.  193,  430. 
735.) 


MERCURIC  BROMIDE 


493 


Solubility  of  HgBr2  in  KBr+Aq  at  25°. 

Mols.  per  liter 


Solubility  in  H2O  at  25°  =  1.4  X  10~7  equiva- 
lents per  1.  (Thompson,  J.  Am.  Chem.  Soc. 
1906,  28.  762.) 

Insol.  in  H2O  and  dil.  acids.  Decomp.  by 
HCl+Aq.  Sol.  in  hot  cone.  H2SO4  with 
evolution  of  SO2.  SI.  sol.  in  hot  HNO3+Aq 
of  1.42  sp.  gr.  (Stromann,  B.  20.  2818.) 

Decomp.  into  Hg  and  HgBr2  by  boiling 
with  NH4Br,  or  NH4Cl+Aq;  also  by  am- 
monium carbonate  or  succinate,  but  not  by 
ammonium  sulphate  or  nitrate.  (Witt- 
stein.) 

Sol.  in  Hg(NO3)2+Aq.  (Wackenroder,  A. 
41.  317.) 

Partially  decomp.  by  alkali  chlorides  +Aq  ; 
when  out  of  contact  of  air  this  decomp.  is 
slight  and  HgBr2  is  formed,  while  in  the  air 
HgCl2  is  the  resulting  product.  Much  more 
rapidly  decomp.  in  hot  than  cold  solutions. 
(Miahle,  A.  ch.  (3)  5.  177.) 

A  solution  of  HgBr  in  0.1 — N  KBr  contains 
about  1  mg.  Hg  ions  in  1300  1. 

Insol.  in  alcohol. 

Insol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1370.) 

Insol.  in  methyl  acetate  (Naumann, 
B.  1909,  42.  3790) ;  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329);  (Eidmann,  C.  C.  1899,  II.  1014.) 

Mercuric  bromide,  HgBr2. 

Sol.  in  250  pts.  H2O  at  ordinary  temp.,  and  25  pts. 
boiling  HoO.  (Wittstein.)  Sol.  in  240  pts.  H2O  at 
18.75°.  (Abl.) 

Sol.  in  94  pts.  H2O  at  9°,  and  in  4-5  pts.  at 
100°.  (Lassaigne,  J.  chim.  med.  12.  177.) 

Solubility  in  g-equivalents  per  litre  = 
2X10-2.  (Bodlander,  Z.  phys.  Ch.  1898,  27. 
61.) 

1  1.  H2O  dissolves  about  4  g.  at  ord.  temp. 
(Morse,  Z.  phys.  Ch.  1902,  41.  731.) 

1  1.  H2O  dissolves  0.017  mol.  at  25°.  (Jan- 
der,  Dissert,  1902.) 

Solubility  in  H2O  at  25°  =  0.017  mol. 
liter.  (Sherrill,  Z.  phys.  Ch.  1903,  43. 
735.) 

Solubility  at  ord.  temp.  =0.8%;  at  bpt. 
8-9%.       (Larine,   J.   Pharm.   1904,    (6)   20. 
450.) 

Solubility  in  cold  H2O=4%,  but  solution 
prepared  by  heating  contains  more  Hg  on 
account  of  decomp.  into  HBr  and  oxybrom- 
ide.  (Vicario,  C.  C.  1907,  II.  1224.) 

1  1.  H2O  dissolves  about  5-6  g.  at  ord. 
temp.  (Gaudechon,  A.  ch.  1911,  (8)  22. 
212.)  • 

1  1.  aqueous  solution  at  25°  contains  0.017 
mol.  (Herz  and  Paul,  Z.  anorg.  1913,  83. 
431.) 

Decomp.  by  warm  HNO3,  or  H2SO4+Aq. 
Sol.  in  warm  H2SO4.  (Ditte,  A.  ch.  (5) 
17. 124.) 

1  mol.  is  sol.  in  1  mol.  warm  HI+Aq.  in 
1  mol.  cold  cone.  HC1  and  in  y%  mol.  hot 
cone.  HC1.  .  (Lowig.) 


KBr 


0. 

0.05 

0.10 

0.5 

0.866 

2 

3 

4 


HgBr2 


0.017 

0.055 

0.088 

0.0359 

0.611 

1.407 

2.096 

2.339 


(Sherrill,  Z.  phys.  Ch.  1903,  43.  705.) 
Solubility  in  various  salts+Aq  at  25°. 


Salt 


NaBr 


KBr 


CaBr2 


SrBr, 


BaBr2 


In  10  ccm.  of  the  solution 


Millimols  Hg  Br2         Millimols  salt 


0.17 

0.78 

2.85 

5.40 

12.76 

15.50 

23.06 


0.17 

0.98 

4.72 

13.60 

19.30 


0.17 
1.17 

6.76 
13.58 
27.66 
36.66 


0.17 

1.04 

4.71 

9.02 

17.70 

22.38 


0.17 
3.70 
5.40 
7.59 
14.78 


0 

1.18 
5.96 
11.42 
24.48 
29.97 
52.46 


0 

2.09 

7.70 

23.80 

34.70 


0 

0.72 

6.45 

18.92 

24.79 

37.54 


0 

0.62 

3.28 

6.68 

14.01 

18.72 


0 

2.74 

3.96 

5.79 

10.96 


(Herz  and  Paul,  Z.  anorg.  1913,  82.  434.) 

Solubility  in  0.1  -N  Hg(NO3)2+Aq  is  about 
20  g.  per  liter.  (Morse,  Z.  phys.  Ch.  1902, 
41.  731.) 

Sol.  in  KBr  or  NaBr+Aq.  (Jander, 
Dissert.  1902.) 

Solubility  in  10  cc.  Br2+Aq  at  25°. 
MillimolBr2          0.753         1.797          2.231 
"      Hg        0.1844       0.1947        0.2120 
(Herz  and  Paul,  Z.  anorg.  1914,  86.  215.) 


494 


MERCURIC  BROMIDE 


Sat.  solution  in  liquid  SO2  contains  about 
1.5%  HgBr2  at  159.4°.  (Niggli,  Z.  anorg. 
1912,  75.  182.) 

Moderately  sol.  in  liquid  NH3.  (Gore, 
Am.  Ch.  J.  1898,  20.  829.) 

Sol.  in  AlBr3.  (Isbekow,  Z.  anorg.  1913, 
84.  27.) 

1  ccm.  of  sat.  solution  in  abs.  alcohol  at 
ord.  temp,  contains  0.0958  g.  HgBr2;  at  bpt. 
contains  0.1262  g.  (Hamper,  Ch.  Z.  1887,  11. 
905.) 

Solubility  of  HgBr2  in  alcohols +Aq  at  t°. 


Alcohol 

t° 

G.  HgBr2  per 
100  g.  alcohol 

Methyl  alcohol 

0 
10 
19 
22 
39 
65 
97 

41.15 
40.5 

66.3 
60.9 
71.3 
90.8 
139.1 

Ethyl  alcohol 

0 
10 
19 
39 
65 
89 

25.2 
26.3 
29.7 
31.9 
44.5 
66.9 

Propyl  alcohol 

0 
10 
19 

39 
65 
86.5 

14.6 
15.6 
15.5 
20.8 
31.3 
42.7 

Isobutyl  alcohol 

0 
10 
23 
39 
65 

4.61 
5.63 
6.65 
9.58 
15.80 

(Timofeiew,  Dissert.  1894.) 

Much  more  sol.  than  HgI2  in  alcohol. 
100  g.  of  solution  sat.  at  0°  contain  13.33- 
13.05  g.  HgBr2;  16.53  g.  at  25°;  22.63  g.  at 
50°.  (Reinders,  Z.  phys.  Ch.  1900,  32.  522.) 

Solubility  of  HgBr2  in  methyl  alcohol +Aq  at 
25°. 

P  =  g.  alcohol  in  100  g.  alcohol +Aq. 

HgBr2  =  millimols.  HgBr2  in  10  cc.  of  the 
solution. 


p 

HgBr2 

Sp.  gr. 

1.0022 
0.9857 
0.9588 
0.9508 

P 

HgBr2 

Sp.  gr. 

0 
10.60 
30.77 
37.21 

0.167 
0.201 
0.358 
0.422 

47.06 
-64.00 
78.05 
100 

0.700 
1.90 
4.07 
13.96 

0.9401 
0.9386 
0.9744 
1.2275 

Solubility  of  HgBr2  in  ethyl  alcohol +Aq  at  25°. 

P  =  g.  alcohol  in  100  g."  alcohol  +Aq. 

HgBr2  =  millimols.  HgBr2  in  10  cc.  of  the 
solution. 


p 

HgBr2 

Sp.  gr. 

0 
20.18 
40.69 
70.01 
100 

0.167 
0.187 
0.440 
1.829 
6.337 

1.0022 
0.9717 
0.9435 
0.9214 
0.9873 

(Herz  and  Anders.) 

Solubility  in  mixtures  of  methyl  and  propyl 
alcohol  at  25°. 
P  =  %  propyl  alcohol  in  the  solvent. 
G  =  g.  HgBr2  in  10  ccm.  of  the  solution. 
S  =  Sp.  gr.  of  the  sat.  solution. 

p 

G 

S  25°/4° 

0 
11.11 
23.8 
65:2 
91.8 
93.75 
96.6 
,  100 

5.02 
4.728 
4.153 
2.530 
1.635 
1.586 
1.466 
1.873 

1.227 
1  .  1954 
1  .  1524 
1.0257 
0.9437 
0.9368 
0.9275 
0.9213 

(Herz  and  Kuhn,  Z.  anorg.  1908,  60.  158.) 

Solubility  in  mixtures  of  ethyl  and  propyl 
alcohol  at  25°. 
P  =  %  propyl  alcohol  in  the  solvent. 
G  =  g.  HgBr2  in  10  ccm.  of  the  solution. 
S  =  Sp.  gr.  of  the  sat.  solution. 

P 

G 

S  25°/4° 

0 
8.1 
17.85 
56.6 
88.6 
91.2 
95.2 
100 

2.28 
2.225 
2.106 
1.763 
1.476 
1.464 
1.406 
1.378 

0.9873 
0.9802 
0.9740 
0.9487 
0.9269 
0.9239 
0.9227 
0.9213 

(Herz  and  Kuhn,  Z.  anorg.  1908,.  60.  161.) 

Solubility  of  HgBr2  in  mixtures  of  methyl  and 

ethyl  alcohol  at  25°. 
P  =  %  methyl  alcohol  in  the  mixtures. 
HgBr2  =g.  HgBr2  in  10  ccm.  of  the  solution. 
S25°  4°  =  sp.  gr.  of  the  sat.  solution. 


(Herz  and  Anders,  Z.  anorg.  1907,  52.  165.) 


P 

HgBr2 

S  25°/4° 

0 

2.28 

0.9873 

4.37 

2.31 

0.9932 

10.4 

2.54 

1.009 

41.02 

3.33 

1.080 

80.69 

4.57 

1.185 

84.77 

4.68 

1.193 

91.25 

4.86 

1.211 

100 

5.02 

1.227 

(Herz  and  Kuhn,  Z.  anorg.  1908,  58.  163.) 

MERCURIC  SODIUM  BROMIDE 


495 


Cold  sat.  solution  in  anhydrous  ether  con- 
tains 0.00567  g.  in  1  cc.;  hot  solution  contains 
0.032  g.  (Hampe,  Ch.  Z.  1887,  11.  905.) 

Solubility  in  organic  solvents  at  18°-20°. 

100  g.  chloroform  dissolve  0.126  g.  HgBr2. 

100  g.  tetrachlormethane  dissolve  0.003  g. 
HgBr2. 

100  g.  bromoform  dissolve  0.679  g.  HgBr2. 

100  g.  ethyl  bromide  dissolve  2.310  g. 
HgBr2. 

100  g.  ethylene  dibromide  dissolve  2.340  g. 
HgBr2. 

(Sulc,  Z.  anorg.  1900,  25.  401.) 

Solubility  in  CS2  at  t°. 


t 

100  pts.  sat.  solution  contain 
pts.  HgBr2 

—10 

0.049 

5 

0.068 

0 

0.087 

+  5 

0.105 

10 

0.122 

15 

0.140 

20 

0.187 

25 

0.232 

30 

0.274 

Mols. 
HgBr2 
per  100 

s 

Mols. 
HgBr2 
per  100 

s 

Mols. 
HgBr2 
per  100 

S 

4.9 

10. 

12.5 
14.9 
19.7 
23.4 

9° 
43.5 
57 
68 
89 
106 

,25.4 
33.9 
39.5 
41.9 
43.9 
46.2 

115.5° 
117 
108 
113 
118 
121 

49.6 

54.9 

58.8 
64.0 

123 
124 
134 
133 

(Staronka,  Anz.  Ak.  Wiss.  Krakau,  1910,  372.) 

Solubility  of  HgBr2  in  quinoline. 

(Arctowski,  Z.  anorg.  1894,  6.  267.) 

100  g.  boiling  methyl  acetate  (bpt.  56.2- 
56.7°)  dissolves  24  g.  HgBr2.  (Schroeder  and 
Steiner,  J.  pr.  1909,  (2)  79.  49.) 

1  g.  HgBr2  is  sol.  in  4.56  g.  methyl  acetate 
at  18°.  Sp.  gr.  18°/4°  of  sat.  solution  =  1.09. 
(Naumann,  B.  1909,  42.  3795.) 

100  g.  anhydrous  ethyl  acetate  or  sat. 
with  H2O  at  18°  dissolve  130.5-135  g. 
HgBr2.  (Hamers,  Dissert.  1906.) 

Solubility  of  HgBr2  in  ethyl  acetate  -f-Aq  at 
25°. 

P  =  g.  ethyl  acetate  in  100  g.  ethyl  acetate 
+Aq. 

HgBr2  =  millimols  HgBr2  in  10  cc.  of  the 
solution. 


p 

HgBr2 

Sp.  gr. 

0 
4.39 
96.76 
100 

0.167 
0.159 

7.42 
3.93 

1.0022 
1.0018 
1.1159 
1.0113 

(Herz  and  Anders,  Z.  anorg.  1907,  62.  172.) 

1  pt.  HgBr2  sol.  in  7.66  pts.  ethyl  acetate 
at  18°.  (Naumann,  B.  1910,  43.  315.) 

Easily  sol.  in  acetone.  (Oppenheim,  B.  2. 
572.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014.) 

Acetone  dissolves  much  more  HgBr2 
than  HgI2.  100  g.  sat.  solution  at  25°  con- 
tain 34.58  g.  HgBr2.  (Reinders,  Z.  phys. 
Ch.  1900,  32.  514.) 


Solubility  in  diethyl  oxalate  is  much  greater 
than  that  of  HgI2  and  is  equal  to  12%  at 
100°.  (Reinders,  Z.  phys.  Ch.  1900,  32.  507.) 

Solubility  in  benzene  =  0.0194  mol.  per 
1.  at  25°.  (Sherrill,  Z.  phys.  Ch.  1903,  43. 
735.) 

Sol.  in  allyl  mustard  oil.  (Mathews,  J. 
phys.  Chem.  1905,  9.  647.) 

Sol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1369.) 

Solubility  in  aniline. 
S  =  temp.  of  solidification. 


S  =  temp.  of  solidification. 
Mols.  HgBr2 

per  100          4.4       8.9         14.3       17.6 
S  88°       111°       127°       134° 

(Staronka,  Anz.  Wiss.  Krakau,  1910.  372.) 

Mol.  weight  determined  in  ethyl  sulphide. 
(Werner,  Z.  anorg.  1897,  15.  30.) 
+4H2O.    (Thomsen.)     , 

Mercuric  perbromide,  HgBr4. 

(Herz  and  Paul,  Z.  anorg.  1914,  85.  216.) 

Mercuric  hydrogen  bromide  (Bromomercuric 

acid),    HgBr2,    HBr  =  HHgBr3. 
Decomp.  by  H2O.    (Neumann,  M.  10.  236.) 

Mercuric    nickel    bromide,    basic,    HgBr2, 

NiBr2,  6NiO+20H2O. 
(Mailhe,  A.  ch.  1902,  (7)  27.  369.) 

Mercuric  platinum  bromide. 
See  Bromoplatinate,  mercuric. 

Mercuric  potassium  bromide,  HgBr2,  KBr. 

Sol.  in  H2O,  but  decomp.  by  a  large  amount, 
with  separation  of  one  half  of  the  HgBr2.  (v. 
Bonsdorff,  Pogg.  19.  339.) 

2HgBr2,  KBr+2H2O.  Permanent.  Sol.  in 
H2O  and  alcohol,  (v.  Bonsdorff.) 

Mercuric  sodium  bromide,  HgBr2,  NaBr. 
Deliquescent,     (v.  Bonsdorff.) 
(Varet,  C.  R.  1890,  111,  527.) 


496 


MERCURIC  SODIUM  BROMIDE 


HgBr2,  2NaBr. 

Very  sol.  in  H2O.  (Vicario,  J.  Pharm. 
1907,  (6)  26..  145.) 

2HgBr2,  NaBr+3H2O.  Sol.  in  H2O  and 
alcohol.  (Berthemot.) 


Mercuric  strontium  bromide,  HgBr2,  SrBr2. 

Sol.  in  all  proportions  of  H2O.  (Lowig, 
Mag.  Pharm.  33.  7.) 

2HgBr2,  SrBr2.  Decomp.  by  H2O  into 
HgBr2  and  HgBr2,  SrBr2.  (Lowig.) 

Mercuric  zinc  bromide. 

Deliquescent  in  moist  air.     (v.  Bonsdorff.) 

Mercuric   zinc   bromide   cyanide   ammonia. 
See  Cyanide  zinc  bromide  ammonia,  mer- 
curic. 

Mercuric  bromide  ammonia,  HgBr2,  2NH3. 
Decomp.  by  boiling  H2O.     Sol.  in  min. 
acids  and  acetic  acid.     (Naumann,  B.  1910, 
43.  316.) 

Mercuric  bromide  cadmium  oxide, 

HgBr2,  CdO+H2O. 
(Mailhe,  A.  ch.  1902,  (7)  27.  371.) 

Mercuric  bromide  cupric  oxide, 

HgBr2,  CuO+3H2O. 
(Mailhe,  Bull.  Soc.  1901,  (3)  25.  791.) 

Mercuric  bromide  hydrazine,  HgBr2,  N2H4. 
(Hofmann   and   Marburg,    A.    1899,    305. 
215.) 

Mercuric  bromide  potassium  chloride, 

HgBr2,  2KC1. 

Decomp.  by  H2O.  (Harth,  Z.  anorg. 
1897,  14.  345.) 

Mercuric  bromide  zinc  oxide,  HgBr2,  ZnO  + 

8H2O. 
(Mailhe,  C.  R.  1901,  132,  1274.) 

Mercuric  bromoiodide,  HgBrl. 

Sol.  in  alcohol  and  ether.  Can  be  recrystal- 
lised  from  ether  without  decomp.  (Oppen- 
heim,  B.  2.  571.) 

Mercurous  chloramide,  Hg2(NH2)Cl. 

Insol.  in  boiling  H2O  or  NH4OH+Aq. 
(Kane,  A.  ch.  (2)  72.  215.) 

Mixture  of  Hg  and  HgNH2Cl.  (Barfoed, 
J.  pr.  (2),  39.  201.) 


Mercuric  chloramide,  Hg(NH2)Cl. 

Composition  is  dimercuriammonium  am- 
monium chloride,  Hg2NCl,  NH4C1,  which 

see. 

Mercuric  chloramide  oxymercuriammonium 
chloride,  4Hg(NH2)Cl,  (NHg2OH2)Cl. 

(Millon.) 

Correct  composition  is  cfomercuriammonium 
ammonium  chloride,  NHg2Cl,  NH4C1,  which 
see.  (Balestra,  Gazz.  ch.  it.  21.  (2)  294.) 

Hg(NH2)Cl,    (NHg2OH2)Cl.      (Millon.) . 

True  composition  is  rfomercuriammonium 
mercuric  chloride,  2Hg2NCl,  HgCl2+H2O; 
or  fKmercuriammonium  hydrogen  chloride, 
NHg2Cl,  HC1.  (Balestra.) 

Mercuric  chloramide  chloride,  Hg(NH2)Cl, 
HgCl2. 

Properties  as  mercuric  chloramide.  De- 
comp. by  cold  HCl+Aq.  (Millon.) 

True  composition  is  dmiercuriammonium 
hydrogen  chloride,  NHg2Cl,  2HC1.  (Ba- 
lestra, Gazz.  ch.  it.  21.  (2)  294.) 

Mercuric     chloramide     chromate, 

2Hg(NH2)Cl,  HgCrO4. 
Decomp.  by  hot  H2O.    Easily  sol.  in  HNO3 
or  HCl+Aq.    (Jager  and  Krtiss,  B.  22.  2048.) 

Mercurous  chloride,  Hg2Cl2. 

Ahnost  absolutely  insol.  in  cold,  but  gradu- 
ally si.  decomp.,  by  boiling  H2O. 

Calculated  from  electrical  conductivity  of 
Hg2Cl2+Aq,  1 1 H2O  dissolves  3.1  mg.  Hg2Cl2 
at  18°.  (Kohlrausch  and  Rose,  Z.  phys.  Ch. 
12.  241.) 

1  1.  H20  dissolves  2  mg.  Hg2Cl2  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1904,  50.  356.) 

1 1.  H2O  dissolves  1.4  mg.  at  0.5°;  21  mg.  at 
18°;  2.8  mg.  at  24.6°;  7  mg.  at  43°.  (Kohl- 
rausch, Z.  phys.  Ch.  1908,  64.  150.) 

When  finely  divided,  is  10%  more  sol.  than 
when  coarsely  crystalline.  (Sauer,  Z.  phys. 
Ch.  1904,  47.  184.) 

Solubility  in  H2O  =  0.8  X 10-6  g.  mol.  (Ley, 
Z.  Elektrochem.  1904,  10.  301.) 

SI.  sol.  with  decomp.  in  boiling  H2O  free 
from  air,  20  ccm.  H2O  affording  0.002  g. 
HgCl2  after  boiling  1  hour  with  Hg2Cl2. 
(Miahle,  A.  ch.  (3)  5.  176.)  Hg2(NO3)2  + 
Aq  containing  1  pt.  Hg2(NO3)2  to  250,000 
pts.  H2O  give  ppt.  of  Hg2Cl2  with  HCl+Aq. 
Sol.  with  decomp.  in  cone.  HCl+Aq,  hot 
HNO3+Aq,  aqua  regia,  or  Cl2+Aq.  (Fre- 
senius.)  Insol.  in  cold  dil.  acids,  but  slowly 
sol.  on  heating. 

The  solubility  of  Hg2Cl2  in  HCl+Aq  in- 
creases slowly  with  time,  and  finally  reaches  a 
point  where  it  increases  very  rapidly,  which 
takes  place  sooner  the  more  dil.  the  acid. 
Presence  of  Hg2(NO3)2+Aq  helps  the  solu- 
bility. (Why  not  oxidation  to  HgCl2?) 
(Varenne,  C.  R.  92.  1161.) 


MERCURIC  CHLORIDE 


497 


Solubility  of  Hg2Cl2  in  HCl+Aq  at  25°. 
Solid  phase  =  Hg2Cl2 +0.1  g.  Hg. 


G.  per  1. 

Sp.  gr.  of 
solutions 

HC1 

HgzCh 

31.69 

0.034 

36.46 

0.048 

95.43 

0.207 

l!042 

158.4 

0.399 

1.069 

209.2 

0.548 

1.091 

267.3 

0.654 

1.114 

278.7 

0.675 

1.119 

317.3 

0.670 

1.132 

364.6 

0.673 

1.153 

(Richards  and  Archibald,  Z.  phys.  Ch.  1902. 
40.  385.) 

Cold  cone.  H2SO4  does  not  dissolve  or 
decomp.  Boiling  H2SO4  dissolves  with  evo- 
lution of  SO2.  (Vogel.) 

Solubility  of  Hg2Cl2  in  chlorides +Aq  at  25°. 
Solid  phase =Hg2Cl2 +0.1  g.  Hg. 


Salt 

G.  pe 

r  liter 

Sp.  gr.  of 

NaCl 

Hg2Cl2 

solutions 

NaCl 

5.85 
58.50 
119. 
148.25 
222.3 
292.5 

0.0041 
0.041 
0.129 
0.194 
0.380 
0.643 

i!6io 

1.078 
1.093 
1.142 

1.188 

BaCl2 

104.15 
156.22 
208.30 
312.54 

0.044 
0.088 
0.107 
0.231 

1.088 
1.134 
1.174 
1.263 

CaCl2 

39.96 
55.5 
111 
138.75 
195.36 
257.52 
324.67 
432.9 
499.5 

0.022 
0.033 
0.081 
0.118 
0.231 
0.322 
0.430 
0.518 
0.510 

!664 
.105 
.151 
.205 
.243 
.315 
1.358 

(Richards  and  Archibald,  Z.  phys.  Ch.  1902, 
40.  385.) 

Sol.  in  cold  HCN+Aq  with  separation  of 
Hg. 

Sol.  in  alkali  chlorides+Aq.  NH4Cl+Aq 
dissolves  out  HgCl2  at  ord.  temp.,  much  more 
at  40-50°.  Dil.  NH4Cl+Aq  decomposes 
more  slowly  than  cone.  Access  of  air  hastens 
reaction.  (Miahle.) 

When  heated  several  hours  to  40-50°,  100 
pts.  NH4Cl+833  pts.  H2O  form  0.75  pt. 
HgCl2  from  25  pts.  Hg2Cl2;  100  pts.  NaCl+ 
833  pts.  H2O  form  0.33  pt.  HgCl2  from  25 
pts.  Hg2Cl2;  100  pts.  KC1+833  pts.  H2O  form 


0.25  pt.  HgCl2  from  25  pts.  HgCl2;  100  pts. 
BaCl2+833  pts.  H2O  form  0.33  pt.  HgCl2 
from  25  pts.  Hg2Cl2.  (Miahle,  J.  Pharm.  26. 
108.) 

Other  chlorides  act  as  NH4C1,  only  less 
vigorously.  (Pettenkofer.) 

By  boiling  1  pt.  Hg2Cl2  10  times  with  a 
solution  of  1  pt.  NaCl  each  time,  the  Hg2Cl2  is 
finally  completely  decomp.  (Henne.) 

Boiling  BaCl2+Aq  or  CaCl2+Aq  dissolve 
traces.  K2SO4+Aq,  KNO3+Aq,  or 
KHC4H4O6+Aq  do  not  dissolve.  (Petten- 
kofer.) 

Sol.  in  (NH4)2SO4+Aq.  Insol.  in  NH4 
nitrate,  or  succinate+Aq.  (Wittstein.) 

Sol.  in  hot  Hg2(NO3)2+Aq,  and  still  more 
in  hot  Hg(NO8)2+Aq;  on  cooling  it  crystal- 
lises out  completely.  25  g.  Hg2Cl2  dissolve  in 
1.5  1.  H2O  containing  50  g.  Hg(NO3)2.  (De- 
bray,  C.  R.  70.  995.) 

Sol.  in  PtCl2+Aq. 

Decomp.  by  NH4OH+Aq. 

Decomp.  by  KOH,  or  NaOH+Aq. 

Sol.  in  Na2S2O3+Aq.  (Faktor,  C.  C. 
1905,  I.  1524.) 

Very  si.  sol.  in  NH4  succinate.  (Witt- 
stein.) 

Insol.  in  SbCl3.     (Klemensiewicz,   C.  C. 

1908,  II.  1850.) 

Very  sol.  in  liquid  NH3.  (Franklin,  Am. 
Ch.  J.  1898,  20.  829.) 

Insol.  in  alcohol  or  ether.  More  sol.  in 
H2O  containing  pepsin  and  an  acid  than  in 
H2O,  and  is  not  converted  thereby  into 
HgCl2.  (Torsellini,  Ann.  Chim.  Ch.  farm. 
(4)  4.  105.) 

Small  amts.  are.  sol.  with  decomp.  in  al- 
cohol, ether  and  CHC13.  1  g.  CHC13  dis- 
solves 0.0046  g.  Hg2Cl2.  (Maclagan,  Arch. 
Pharm.  1884,  222,  788.) 

Formic  acid  (95%)  dissolves  at  16.5°, 
0.02%;  at  18°,  0.0003%.  (Aschan,  Ch.  Z. 
1913,  37.  1117.) 

Insol.  in  methyl  acetate     (Naumann,  B. 

1909,  42.   3790);   ethyl  acetate.      (Hamers, 
Dissert.  1906;  Naumann,  B.  1904,  37.  3602.) 

Somewhat  sol.  in  hydroxylamine  hydro- 
chloride.  (Adams,  Am.  Ch.  J.  1902,  28. 1216.) 

Insol.  in  benzonitrile.  (Naumann,  B/.  1914, 
47.  1370.) 

Insol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

Solubility  in  organic  solvents  at  18-20°. 

100  g.  chloroform  dissolve  traces  of  HgCl. 

100  g.  bromoform  dissolve  0.055  g.  HgCl. 

100  g.  ethyl  bromide  dissolve  traces  of 
HgCl. 

100  g.  ethylene  dibromide  dissolve  traces  of 
HgCl.  (Sulc.  Z.  anorg.  1900,  25.  401.) 

Mercuric  chloride,  HgCl2. 
Permanent. 

Sol.  in  18.5  pts.  H2O  at  13.8°,  and  2-3  pts.  at  100°. 
(J.  Davy,  1822.)  Sol.  in  3  pts.  boiling  H2O.  (Wenzel.) 
Sol.  in  18.23  pts.  IPO  at  10°,  and  3  pts.  at  100°.  (M.  R. 
and  P.)  Sol.  in  18.46  pts.  at  18.75°.  (Abl.)  Sol.  in  16 
pts.  cold,  and  3  pts.  warm  HjO.  (Dumas.) 


498 


MERCURIC  CHLORIDE 


100  pts.  H2O  dissolve  pts.  HgCl2  at  t°: 


t° 

Pts. 
HgCh 

t° 

Pts. 
HgCU 

t° 

Pts. 
HgCb 

0 
10 
20 
30 

5.73 
6.57 
7.39 
8.43 

40 
50 
60 
70 

9.62 
11.34 
13.86 
17.29 

80 
90 
100 

24.30 
37.05 
53.96 

(Poggiale,  A.  ch.  (3)  8.  468.) 


Solubility  of  HgCl2  in  H2O. 


t 

%  HgCl2 

t 

%  HgCl2 

+  1 

3.9 

80 

23.6 

4.5 

4.8 

87 

28.2 

4.5 

4.8 

100 

39.3 

7.5 

5.1 

121 

59.7 

13.8 

5.2 

127 

69.7 

25.1 

7.1 

140 

77.0 

29.5 

7.6 

150 

78.4 

38.0 

9.9 

159 

80.2 

49 

11.3 

160 

81.7 

61 

15.1 

165 

81.8 

(Etard,  A.  ch.  1894,  (7)  2.  557.) 


71.17  g.  HgCl2  are  sol.  in  1  1.  H2O  at  25°. 
(Morse,  Z.  phys.  Ch.  1902,  41.  726.) 

Solubility  at  25°  =  0.267  mol.  in  1  1.  H2O. 
(Jander,  Z.  Elektrochem.  1903,  8.  688.) 

Solubility  in  H2O  at  25°  =  0.263  mol.  liter. 
(Sherrill,  Z.  phys.  Ch.  1903,  43.  735.) 

Sat.  HgCl2+Aq  at  25°  contains  6.9% 
HgCl2.  (Foote,  Am.  Ch.  J.  1906,  35.  238.) 

HgCl2+Aq  contains  3.95  g.  HgCl2  in  100  g. 
of  solution  at  0°;  7.67  g.  at  30°.  (Schreine- 
makers,  Ch.  Weekbl.  1910,  7.  202.) 

HgCl2+Aq  sat.  at  (?)  contains  6.8% 
HgCl2.  (Abe,  J.  Tok.  Chem.  Soc.  1912,  33. 
1087.) 

HgCl2+Aq  sat.  at  35°  contains  8.51% 
HgCl2.  (Schreinemakers  and  Thonus,  Ver. 
K.  Akad.  Wet.  Amsterdam,  1912,  21.  333.) 

1  1.  aqueous  solution  sat.  at  25°  contains 
0.265  mol.  HgCl2.  (Herz  and  Paul,  Z.  anorg. 
1913,  82.  431.) 

H2O  dissolves  7.39%  at  20°.  (Aschan, 
Ch.  Z.  1913,  37.  1117.) 


HgCU+Aq  sat.  at  8°  has  1.041  sp.  gr.      (Anthon, 

Sp.  gr.  of  HgCl2+Aq  at  20°. 


%  HgCU 

Sp.  gr. 

%  HgCl2 

Sp.  gr. 

1 

2 
3 

1.0072 
1.0148 
1.0236 

4 
5 

1.0323 
1.0411 

(Schroder,   calculated  by  Gerlach,  Z.   anal. 
27.  306.) 


Sp.  gr.  of  HgCl2+Aq  at  15°. 


%  HgCl2 

Sp.  gr. 

%  HgCU 

Sp.  gr. 

8 
9 
10 

1.071 
1.0815 
1.095 

11 

12 
13 

1  .  1035 
1.115 
1.127 

(Mendeleieff,  calculated  by  Gerlach,  Z.  anal. 
27.  306.) 


Sp.gr.  of  HgCl2+Aq. 


HgCl2 

Sp.  gr. 

at  0° 

at  lb° 

at  20° 

at  30° 

4.72 
3.57 
2.42 
1.22 

1.04070 
1.03050 
1.02035 
1.01008 

1.04033 
1.03022 
1.02018 
1.00990 

1.03856 
1.02885 
1.01856 
1.00835 

1.03566 
1.02577 
1.01585 
1.00575 

(Schroder,  B.  19.  161  R.) 

Sp.  gr.  of  HgCl2+Aq  at  room  temp,  con- 
taining: 

0.226  3.55%  HgCl2. 

1.0233  1.0328 

(Wagner,  W.  Ann.  1883,  18.  266.) 

Sp.  gr.  of  HgCl2+Aq  at  25°. 


Concentration  of  HgCU  +Aq. 

Sp.  gr. 

1  /4-normal 

l/8_          « 

1.0275 
1.0138 

(Wagner,  Z.  phys.  Ch.  1890,  6.  39.) 

Sp.  gr.  at  16°/4°  of  HgCl2+Aq  containing 
4.5256%  HgCl2  =  1.03806. 

Sp.  gr.  at  16°/4°  of  HgCl2+Aq  containing 
4.2224%  HgCl2  =  1.03491.  (Schonrock,  Z. 
phys.  Ch.  1893,  11.  768.) 

HgCl2+Aq  containing  6.04%  HgCl2  has 
sp.  gr.  20°/20°  =  1.0523. 

HgCl2+Aq  containing  6.08%  HgCl2  has 
sp.gr.  20° /20°  =  1.0526. 

(Le  Blanc  and  Rohland,  Z.  phys.  ch.  1896, 
19.  282.) 

Sat.  HgCU+Aq  boils  at  101.1°.     (Griffiths.) 

B.-pt.  of  HgCl2+Aq 


%  HgCU 

B.-pt. 

%  HgCU 

B.-pt. 

4.8 
9.0 

100.10° 
100.16 

11.04 
15.2 

100.20° 
100.275 

(Skinner,  Chem.  Soc.  61.  340.) 

Solubility  in  HCl+Aq  is  greater  than  in  H2O. 
(Dumas.) 

Sol.  in  0.5  pt.  HCl+Aq  of  1.158  sp.  gr.  at  23.3°,  form- 
ing a  solution  of  2.412  sp.  gr.  (Davy,  1822.) 


MERCURIC  CHLORIDE 


499 


Solubility  of  HgCl2  in  HCl+Aq. 

Solubility  of  HgCl2  in  NH4Cl+Aq 

Pts.  HCl 
in  100  pts. 
H29 

Pts.  HgCl2 
dissolved 
by  100  pts. 
liquid 

Pts.  HCl 
in  100  pts. 
H20 

Pts.  HgCl2 
dissolved 
by  100  pts. 
liquid 

at  30°.  —  Continued. 

Composition  of  liquid 
phase 

Solid  phase 

0.0 
5« 

6.8 

A(\    C 

21.6 

Q1     A 

127.4 

mQ 

HgCl2 

NH!CI 

%  H20 

10.1 

73.7 

50.0 

148.0 

55.55 

15.94 

28.51 

HgCl2>  NH4C1,  H20 

13.8 

87.8 

68.0 

154.0 

55.85 

15.35 

28.80 

" 

en    71 

M99 

on    ryr 

ii 

(Ditte,  A.  ch.  (5)  22.  551.) 

57.04 

14.10 

28.86 

HgCl2,  NH4C1,  Hv-0  + 

56.98 

14.14 

28.88 

3HgCl2>  2NH4C1,  H20 

Solubility  in  HCl  +  Aq  at  0°.    ^y^  =  ^mols. 

56.83 
56.26 

13.90 
13.04 

29.27 
30.70 

SHgCh,  2NH4C1,  H2O 

HgCl2  (in  mgs.)  in  10  ccm.  solution;  HCl 
=  mols.   HCl   ditto;    H2O=grms.    H2O 
present 

56.43 
56.70 
57.05 

11.88 
11.05 
9.92 

31.69 
32.23 
33.02 

« 

58  55 

9  23 

32  22 

" 

HgCh 

HCl. 

Sp.  gr. 

H2O 

58.65 

9.20 

32.15 

/  SHgClj,  2NH4C1,  H2O  + 
{      9HgCl2,  2NH4C1 

* 

51.83 

8.76 

39.41 

9HgCl2,  2NH4C1. 

9.7 
19.8 
35.5 
55.6 
68.9 
72.37 
85.5 
88.65 

4.3 
9.9 
17.8 
26.9 
32.25 
34.25 
41.5 
48.1 

1.117 
1.238 
1.427 
1.665 
1.811 
1.874 
2.023 
2.066 

9.704 
9.340 
9.816 
8.135 
7.714 
7.679 
7.131 
6.893 

46.00 
39.02 
35.60 
35.10 
32.90 
29.65 
40.12 
21.00 

7.52 
6.28 
5.26 
5.18 
5.06 
3.62 
5.13 
2.29 

46.48 
54.70 
59.14 
59.72 
62.04 
66.73 
54.75 
76.71 

9HgCl2)2NH4Cl+HgCl2 
HgCh 

95.675 

70.  875  . 

2.198 

6.431 

7.67 

0 

92.33 

(Engel,  A.  ch.  (6)  17.  362.) 
Not  decomp.  by  H2SO4  or  HNO3+Aq. 

Sol.  in  630  pts.  H2SC>4,  and  in  more  than  500  pts.  hot 
HNOs+Aq  of  1.41  sp.  gr.  without  decomp.  (J.  Davy.) 

Sol.  in  H2SO4,  HNO3,  HIO3,  or  H2CrO4 
without  decomp.  (Millon,  A.  ch.  (3)  18.  373.) 

Very  si.  sol.  in  HNO3,  but  not  decomp. 
thereby.  (Wurtz.) 

Solubility  of  HgCl2  in  NH4Cl+Aq  at  30°. 


Composition  of  liquid 
phase 

Solid  phase 

% 
HgCl2 

N&Jl 

%H20 

0 

29.5 

70.5 

NH4C1 

15.68 

27.56 

56.76 

11 

22.80 

26.91 

50.29 

" 

31.96 

26.16 

41.88 

" 

42.45 

25.05 

32.50 

** 

50.05 

24.79 

25.16 

(NH4Cl+HgCl2,  2NH4C1, 
1          H20 

50.60 

24.31 

25.09 

HgCh,  2NHiCl,  H20 

53.08 

22.77 

24.15 

•« 

55.97 

21.42 

22.61 

«. 

58.91 

20.06 

21.03 

HgCh,  2NH4C1,  H2O  + 

58.89 

19.98 

21.13 

HgCh,  NH4C1,  H20 

56.83 

18.86 

24.61 

HgCh,  NH4C1,  H20 

56.38 

18.50 

25.12 

" 

55.83 

17.70 

26.47 

« 

55.70 

17.13 

27.17 

«. 

55.58 

16.82 

27.60 

-» 

1  pt.  sat.  NaCl+Aq  dissolves  1.29  pts. 
HgCl2  at  14°.  (Voit,  A.  104.  354.) 

Sat.  NaCl  +Aq  (20  grains  H2O  +7  grains  NaCl)  dis- 
solves 32  grains  HgCh  at  15.5°,  and  3  grains  more  on 
warming.  Sp.  gr.  of  solution  =2.14.  (Davy,  1822.) 

Sat.  KCl+Aq  (21  grains  H2O+7  grains  KC1)  dis- 
solves 8  grains  HgCl2  on  being  gently  heated.  (Davy.) 

Sat.  BaCl2  +Aq  (20  grains  H2O  +8.7  grains  BaClz  + 
2H2O)  dissolves  16  grains  HgCl2  at  15.5°,  and  4  grains 
more  on  heating.  Sp.  gr.  of  solution  =1.9.  (Davy.) 

MgCl2+Aq  (31  grains  HCl+Aq  of  1.58  sp;  gr. 
neutralised  with  MgO)  dissolves  40  grains  HgCl2,  and 
25  grains  more  on  gently  heating.  Sp.  gr.  of  solution  = 
2.83.  (Davy.) 

Sol.  in  sat.  KC1,  NaCl+Aq,  and  in  MnCl2,  ZnCl2, 
CoCl2,  FeCl2,  NiCl2,  and  CuCl2+Aq.  (v.  Bonadorff, 
Pogg.  17.  123.) 


The  solubility  in  H2O  is  greatly  increased 
by  the  addition  of  cupric  chloride.  8.5% 
HgCl2  is  sol.  in  pure  H2O  and  52.8%  HgCl2 
is  sol.  in  18.06%  CuCl2+Aq.  (Schreine- 
makers,  C.  C.  1913,  I.  1858.) 


500 


MERCURIC  CHLORIDE 


Solubility  of  HgCl2+KCl  at  25% 


Composition          Composition  of 
of  solution         undissolved  residue 


% 

KC1 


26.46 
26.24 

26.23 
26.33 
26.33 
23.74 

22.36 
21.39 
20.32 


20.26 
17.85 

9.26 

7.80 
6.84 
6.66 
6.52 


6.64 
6.27 

5.77 
4.68 

4.66 

4.69 

0 


HgCh 


0 
15.04 

15.02 
15.02 
14.92 
18.91 

21.39 

23.88 
27.62 


27.38 
25.34 

18.95 
19.56 
22  81 
24.32 
25.13 


25.16 
25.11 

24.73 
24.75 

25.17 

24.82 
6.90 


100 


34.61 


34.77 
34.05 


21.89 

21.02 
20.76 
20.75 
20.54 


12.09 
11.87 


% 
HgCb 


0 
3.63 

26.15 
52.01 
61.04 
61.66 

62.02 
61.84 
65.24 


73.98 
75.10 

73.36 
73.06 
74.54 
73.99 
76.46 


80.60 
83.20 

83.18 
84.46 

93.58 
98.50 
100 


3.73 


3.21 
3.35 


3.01 

5.62 
6.18 
4.71 
5.47 


4.71 
4.95 


Solid  phase 


KC1 

KC1+2KC1, 
HgCh,  H20 


2KC1,  HgCh 
H20 


2KC1,  HgCl2 

H2O+KC1, 

HgCh,H20 

KC1,  HgCl2, 
H20 


KC1,  HgCl2, 
HiO+KCl, 
2HgCh,(  2H2O 

KC1,  2HgCl2, 
2H2O 

KC1,  2HgCl2, 
2H2O+HgCh 


HgCh 


(Foote  and  Levy,  Am.  Ch.  J.  1906,  35.  239.) 
Solubility  of  |HgCl2+KCl  at  20°. 


G.  per  100  g.  H2O 


0 

1.12 
2.39 
4.05 
4.84 
5.60 
6.71 
7.39 
7.46 
8.95 
15 

17.57 
20.35 
26.31 
30.32 
34.12 
34.18 
34.34 
34.54 
37.72 
41.13 
39.66 
37.87 
35.32 


HgCh 


7.39 
11.63 
15.72 
22.17 
25.16 
25.13 
25.66 
26.41 
24.70- 
19.93 
22.87 
26.12 
29 

34.83 
39.10 
42.82 
39.34 
35.16 
30.63 
24.30 
19.33 
15.76 
10.28 

2.1 


Solid  phase 


HgCl2 


HgCl2+2HgCl2,  KC1 

2HgCl2,  KC1 

a 

2HgCl2,  KCl+HgCl2,  KC1 
/HgCl2,  KC1 


HgCl2,  KCl+HgCl2,  2KC 
HgCl2,  2KC1 


HgCl2,  2KC1+KC1 

KC1 
u 


(Tichomiroff,  J.  russ.  Phys.  Chem.  Soc.  1907 
39.  731.) 


Solubility  of  HgCl2+RbCl  in  H20.  Solu- 
)ility  data  are  given  showing  double  salts 
ormed  at  25°.  (Foote  and  Levy,  1.  c.) 

Solubility  in  NaCl+Aq.  100  pts.  NaCl+Aq 
containing  given  %  .NaCl  dissolve  g. 
HgCl2. 


%  NaCl 


26 
25 
10 

5 

1 

0.5 


g.  HgCh 
at  15° 


128 
120 
58 
30 
14 
10 


g.  HgCh 
at  65° 

152 
142 

68 

36 

18 

13 


g.  HgCh 
at  100° 

208 

196 

110 

64 

48 

44 


Homeyer  and  Ritsert,  Pharm.  Ztg.  33.  738.) 
Solubility  of  HgCl2+NaCl  at  25%. 


Composition 
of  solution 


26.5 
18.66 

18.71 
18.64 
18.87 
14.97 

14.03 
13.25 
13.17 
12.97 

13.14 
13.15 


% 
HgCh 

0 
51.35 

51.32 
51.42 
51.26 
57.74 

59.69 
62.16 
62.59 
62.50 

62.48 
62.55 


Composition  of 
undissolved  residue 


100 


16.38 

16.36 
16.16 
15.96 


% 
HgCh 


0 
16.39 

21.98 
65.45 
71.25 
74.18 

74.21 
74.70 
74.76 
78.20 

88.64 
90.83 


9.44 

9.43 
9.14 
9.28 


Solid  ph£ 


NaCl 

NaCl+NaCl, 
HgCh,  2H20 


NaCl,  HgCh, 
2H20 


NaCl,  HgCh, 
2H2O+HgCh 


(Foote  and  Levy,  Am.  Ch.  J.  1906,  36.  239.) 

105.0  g.  HgCl2  are  sol.  in  1  1.  of  0.1-N 
Hg(NO3)2+Aq  at  25°.  (Morse,  Z.  phys.  Ch. 
1902,  4  .  726.) 

Solubility  in  MCl+Aq  at  25°. 


Salt 


LiCl 


NaCl 


In  10  ccm.  of  the  solution 


Millimols  HgCh 


2.65 

3.51 

6.66 

10.21 

16.78 

22.14 

28.96 

30.62 


2.65 

3.72 

5.08 

7.48 

11.92 

20.22 

27.54 

34.34 


Millimols  salt 


0 

4.14 
8.35 
12.71 
17.38 
22.65 
30.91 
35.27 


0 

2.12 

4.16 

6.71 

11.53 

19.41 

27.83 

31.62 


MERCURIC  CHLORIDE 


501 


Solubility  in  MCl+Aq  at  25°.—  Continued. 

16.2  mols.  methyl,  12.4  mols.  ethyl,  and  18 
mols.   propyl  alcohol  at  20°;   in  6.8   mols. 
methyl,    10.6   mols.    ethyl,    and    14.6   mols. 
propyl  alcohol  at  38.2°.     (Timofejew,  C.  R, 
112.  1224.) 
100  pts.  absolute  methyl  alcohol  dissolve 
66.9  pts.  HgCl2  at  25°;  100  pts.  absolute  ethyl 
alcohol  dissolve  49.5  pts.  HgCl2  at  25°.    (de 
Bruyn,  Z.  phys.  Ch.  10.  783.) 

At  15°,  1  pt.  by  weight  is  sol.  in:  — 
13.53  pts.  H2O. 
1.5       "  methyl  alcohol  of  sp.  gr.  0.7990 
2.5       "  ethyl           "      "     "     "  0.8100 
6.3       "  propyl        "      "     "     "  0.8160 
(Rohland,  Z.  anorg.  1899,  18.  328.) 

100  g.  HgCl2+CH3OH  contain  1.2  g.  HgCl2 
at  the  critical  temp.    (Centnerszwer,  Z.  phys. 
Ch.  1910,  72.  437.) 

Solubility  of  HgCl2  in  methyl  alcohol  +Aq 
at  25°. 
P  =  g.  alcohol  in  100  g.  alcohol  -f-Aq. 
HgCl2  =  millimols  HgCl2  in  10  cc.  of  the 
solution. 

Salt 

In  10  com.  of  the  solution 

Millimols  HgCh 

Millimols  salt 

KC1 

2.65 

3.55 
3.81 
8.36    . 

0 

1.74 
2.21 
6.83 

MgCl2 

2.65 
3.74 
7.19 
11.31 
18.64 
25.69 
32.06 

0 
1.68 
4.15 
5.70 
9.97 
13.20 
17.28 

CaCl2 

2.65 
3.64 
7.66 
11.08 
18.11 
26.45 
33.04 

0 
1.90 
4.02 
6.56 
9.64 
14.29 
17.23 

SrCl2 

2.65 
3.15 
5.63 
8.29 
13.42 
17.76 
22.93 

0 
1.64 
3.11 
5.19 
7.24 
10.46 
13.86 

p 

HgCl2 

Sp.  gr. 

0 
10.60 
30.77 
37.21 
47.06 
64.00 
78.05 
100 

2.67 
2.92 
4.18 
4.96 
7.27 
14.19 
21.11 
17.95 

1.0565 
1.0441 
1.0420 
.0507 
.0809 
.2015 
.3314 
.2160 

BaCl2 

2.65 
6.97 
11.67 
16.20 
26.45 
53.48 

0 
3.85 
5.72 
7.76 
13.36 
30.30 

/"ET/vprr    n-nrl     A-n/^ofo      *?.      a-nrwer      1  QflT      KO      1AK    \ 

(Herz  and  Paul,  Z.  anorg.  1913,  82.  433.) 

Solubility  in  H2O  is  increased  by  presence 
of  I2.  (Herz  and  Paul,  Z.  anorg.  1914,  85. 
214.) 

Solubility  in  H2O  is  increased  by  presence 
of  hydroxylamine  hydrochloride.  (Adams, 
Am.  Ch.  J.  1902,  28.  213.) 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  829.) 

Insol.  in  liquid  CO2.  (Biichner,  Z.  phys. 
Ch.  1906,  64.  674.) 

Abundantly  sol.  in  H2PtCl4+Aq.  (Nilson, 
B.  1876,  9.  1146.) 


100  cc.  90%  ethyl  alcohol  dissolve  27.5°  g. 
HgCl2  at  15.5°.  Sp.  gr.  15°  of  sat.  solution  = 
1.065.  (Greenish  and  Smith,  Pharm.  J.  1903, 
71.  881.) 

100  g.  99.2%  ethyl  alcohol  dissolve  33.4  g. 
HgCl2  at  25°.  (Osaka.) 


Solubility  of  HgCl2  in  ethyl  alcohol +Aq  at 
25°. 

P  =  g.  alcohol  in  100  g.  alcohol +Aq. 

HgCl2=  millimols  HgCl2  in  10  cc.  of  the 
solution. 


Sol.  in  2.5  pts.  cold  alcohol  (Richter)  ;  3  pts.  (Karl)  ; 

2.5  pts.   alcohol  of  0.833   sp.   gr.   at   ordinary   temp., 
and  1.167  pts.  on  boiling  (Berzelius)  ;  2  pts.  alcohol  of 

p 

HgCh 

Sp.  gr. 

0.816  sp.  gr.   at   15.5   (sp.  gr.  of  solution  =1.08)      (J. 
Davy,  Phil.  Trans.  1822.  358). 

0 

2.67 

1.0565 

At  10°,  sol.  in  2.57  pts.  alcohol  of  39°  (Cartier),  in 

20  18 

2  49 

1  0214 

2.9  pts.  alcohol  of  38°;  in  3.6  pts.  alcohol  of  35°;  in  4.2 
pts.  alcohol  of  30°;  in  9.3  pts.  alcohol  of  22°;  in  14.6  pts. 
alcohol  of  14°.     (N.  E.  Henry.) 

40^69 
70.01 

3^94 
8.70 

i!oiso 

1.0616 

100 

13.61 

1  .  1067 

Sol.  in  25  mols.  methyl    13.1  mols.  ethyl 

and  20.3  mols.  propyl  alcohol  at  8.5°;  in 

(Herz  and  Anders,  Z.  anorg.  1907,  62.  170.) 

502 


MERCURIC  CHLORIDE 


Solubility  of  HgCl2  in  ethyl  alcohol +Aq 
at  25°. 


%  C2H6OH 

%  HgCl2 

%  C2H5OH 

%  HgCh 

0 

6.80 

45.84 

15.36 

5.08 

6.65 

49.86 

18.18 

14.49 

6.41 

53.61 

21.40 

21 

6.55 

57.26 

24.51 

26.25 

7.31 

60.55 

27.67 

31.53 

8.51 

63.95 

29.86 

36.85 

10.32 

67.39 

32.40 

41.36 

12.69 

(Abe,  J.  Tok.  Chem.  Soc.  1912,  33.  1087.) 


Solubility  in  alcohol  is  increased  by  presence 
of  hydroxylamine  hydrochloride.  (Adams, 
Am.  Ch.  J.  1902,  28.  213.) 


Solubility  of  HgCl2  in  a  mixture  of  methyl 
and  ethyl  alcohol  at  25°. 

P  =  %  methyl  alcohol  in  the  mixture. 
HgCl2  =  g.  HgCl2  in  10  ccm.  of  the  solution. 
S=sp.  gr.  of  the  sat.  solution. 


C 

4.37 
10.4 
41.02 
80.69 
84.77 
91.25 
100 


HgCl2 


3.686 
3.943 
4.261 
5.837 
6.167 
5.782 
5.385 
4.862 


S  25°/4c 


107 
130 
157 
294 


1.321 


288 
254 
216 


(Herz  and  Kuhn,  Z.  anorg.  1908,  58.  161.) 


Solubility  in  mixtures  of  methyl  and  propy 
alcohol  at  25°. 


P=%pro 


1  alcohol  in  the  solvent. 

2  in  10  ccm.  of  the  solution. 


S  =  Sp.  gr.  of  the  sat.  solution. 


P 

G 

S  25°/4° 

0 

4.862 

1.2160 

-  11,11 

—5,03^ 

1.2278 

23.8 

5.714 

1.2848 

65.2 

4.228 

1.1568 

91.8 

2.509 

1.0090 

93.75 

2.323 

1.0029 

96.6 

2.152 

0.9851 

100 

2.003 

0.9720 

(Herz  and  Kuhn,  Z.  anorg.  1908,  60.  157.) 

olubility  in  mixtures  of  propyl  and  ethyl 

alcohol  at  25°. 

P  =  %  propyl  alcohol  in  the  solvent. 
G  =  g.  HgCl2  in  10  ccm.  of  the  solution. 
S  =  Sp.  gr,  of  the  sat.  solution. 


0 

8.1 
17.85 
56.6 
88.6 
91.2 
95.2 
100 


3.686 
3.667 
3.406 
2.711 


166 
160 

087 


2.003 


S  25°/4° 


1.1070 
1.0988 
1.0857 
1.0272 
0.9854 
0.9824 
0.9772 
0.9720 


(Herz  and  Kuhn,  Z.  anorg.  1908,  60.  160.) 
Sp.  gr.  of  HgCl2+alcohol. 


%  HgClz 


0 

5.44 

6.52 


Sp.  gr.  25°/20° 


0.7948 
0.8346 
0.8431 


(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  283.) 

Sp.  gr.  of  alcoholic  solution  of  HgCl2. 


HgCb 


0.00 

1.22 

2.38 

4.42 

8.56 

12.43 

15.91 

19.32 

22.46 


Sp.  gr. 


at  0° 


0.83135 

0.8397 

0.8484 

0.8635 

0.8966 

0.9306 

0.9629 

0.9951 

1.0285 


at  10° 


0.82286 

0.8312 

0.8399 

0.8549 

0.8877 

0.9213 

0.9523 

0.9852 

1.0184 


at  20° 


0.81435 

0.8228 

0.8314 

0.8463 

0.8789 

0.9119 

0.9425 

0.9753 

1.0083 


at  30° 


0.80594 

0.8141 

0.8227 

0.8375 

0.8689 

0.9024 

0.9329 

0.9652 

0.9982 


(Schroder,  B.  19.  161  R.) 

Sp.  gr.  at  16°/4°  of  HgCl2+ethyl  alcohol 
containing  23.5489%  HgCl2=  0.99885;  con- 
taining 11. 8801%  =0.88572.  (Schonrock,  Z. 
phys.  Ch.  1893,  11.  768.) 

Sp.  gr.  at  16°/4°  of  HgCl2+amyl  alcohol 
containing    10.9948%    HgCl2  =  0.89550. ' 
(Schonrock,  Z.  phys.  Ch.  1893,  11.  769.) 

Sol.  in  4  pts.  ether  (Karls);  in  4.1  pts. 
(Henry);  in  2.86  pts.  ether  of  0.745  sp.  gr. 
(sp.  gr.  of  solution  =  1.08);  the  solvent  power 
is  not  increased  by  elevating  the  temp.,  and 
b.-pt.  of  ether  is  not  raised.  (J.  Davy.) 

Ether  extracts  HgCl2  from  HgCl2+Aq. 
(Orfila);  very  slightly  if  HgCl2+Aq  is  dil. 
(Lassaigne.) 

Very  si.  sol.  in  pure  ether.     (Polis,  B.  20. 

6.35  pts.  are  sol.  in  100  pts.  ether  at  0°. 

6.44     "     "     "     "  100    "      "      "   18. 

6.38     "    "     "  -"  100    "      "      "  35.5. 

(Laszczynski,  B.  18.94,  27.  2286.) 


MERCURIC  CHLORIDE 


503 


Sol.  in  7J4-8  pts.  ether.  (Madsen,  Ch.  Z. 
Repert.  1897,  21.  169.) 

Solubility  in  100  cc.  ether  at  17°  =  4.1-4.12 
g.  (Stromholm,  J.  pr.  1902,  (2),  66.  450.) 

The  solubility  of  HgCl2  in  H2O  is  only  si. 
affected  by  the  presence  of  ether.  An  aqueous 
solution  sat.  with  ether  and  HgCl2  contains 
about  10%  less  HgCl2  than  a  pure  sat. 
aqueous  solution.  Partition  coefficient  for 

=  4.9  at  0°;  3.02  at  14.6°;  2.80  at 

16.8°.  "(Stromholm,  Z.  phys.  Ch.  1903,  44. 

70.) 


126.80  pts.  HgCl2  are  sol.  in  100  pts.  acetone 
at  18°.  (Lasczynski,  B.  1894,  27.  2287.) 

1  g.  HgCl2  is  sol.  in  0.70  g.  acetone  at  18-°. 
gr.  of  sat.  solution  18°/4°  =  1.956.) 
(Naumann,  B.  1904,  37.  4334.) 

Sat.  solution  in  acetone  contains  57.74  g. 
HgCl2  in  100  g.  solution  at  25°.  (Foote  and 
Haigh,  J.  Am.  Chem.  Soc.  1911,  33.  461.) 

Sp.  gr.  at  26.7°/4°  of  HgCl2+acetone  con- 
taining 36.25%  HgCl2- 1.1585.  (Schonrock, 
Z.  phys.  Ch.  1893,  11.  769. 


Sp.  gr.  of  HgCl2+ acetone. 


Solubility  of  HgCl2  in  ether+Aq  at  25°. 

%  Ether 

%  H2O 

%  HgCl2 

87.86 
1.2 
5.2 
5.4 
5.4 

5.22 
93.6 
90.5 
91.8 
93.1 

6.92 
5.2 
4.3 

2.8 
1.5 

%  HgCl2 

Sp.  gr.  20°/20° 

0 
10.94 
21.05 

0.8003 
0.8847 
0.9799 

(Abe,  J.  Tok.  Chem.  So,c.  1912,  33.  1087.) 


(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896. 
19.  283.) 

100  g.  methyl  acetate  dissolve  46  g.  at 
bpt.  (56.5°).  (Schroeder  and  Steiner,  J.  pr. 
1909,  (2)  79.  49.) 

1  g.  HgCl2  is  sol.  in  2.35  g.  methyl  acetate 


at  25°. 

at  18°.    Sp.  gr.  18°/4°  of  the  sat.  solution  = 
1.251.    (Naumann,  B.  1909,  42.  3793.) 

Solubility  in  ethyl  acetate. 

%  Alcohol 

%  IigCl2 

'   %  Alcohol. 

%  HgCh 

67.57 
58.59 
51.02 
44.79 
38.69 
32.84 

32.43 
32.50 
37.39 
37.96 
38.24 
37.75 

27.16 
22.48 
15.20 

8.97 
0 

36.29 
34.08 
28.55 
20.67 
5.49 

Pts.  sol.  in  100  pts.  ethyl 

acetate. 

Pts.  HgCl2 

t°   , 

28.92 
29.03 
30.71 
31.87 
32.77 
35.98 

0 
13 
35 
48 
60 
83 

(Abe.) 

4  pts.  ether  dissolve  1  pt.  HgCl2,  but  4 
pts.  ether  +1.33  pts.  camphor  dissolve  1.33 

pts.  HgCl2;  4  pts.  ether +4  pts.  camphor  dis- 
solve 2  pts.  HgCl2;  4  pts.  ether +8  pts.  cam- 
phor dissolve  4  pts.  HgCl2;  4  pts.  ether +16 
pts.  camphor  dissolve  8  pts.  HgCl2.  (Karls, 
Pogg,  10.  608.) 

3  pts.  alcohol  dissolve  1  pt.  HgCl2,  but  3 
pts.  alcohol +1  pt.  camphor  dissolve  2  pts. 
HgCl2;  3  pts.  alcohol +3  pts.  camphor  dis- 
solve 3  pts.  HgCl2;  3  pts.  alcohol+6  pts. 
camphor  dissolve  6  pts.  HgCl2.  (Karls,  I.  c.) 

Solution  can  be  obtained  containing  25  pts. 
camphor,  16  pts.  HgCl2,  and  only  4  pts. 
alcohol.  Sp.  gr.  of  solution  =  1.326.  (Simon, 
Pogg.  37.  553.) 

100  pts.  acetone  dissolve  60  pts.  HgCl2  at 
25°.  (Krug  and  M'Elroy,  J.  Anal.  Appl.  Ch. 
184.) 

9836  pts.  HgCl2  are  sol.  in  100  pts.  acetone 
atO°. 

110.95  pts.  HgCl2  are  sol.  in  100  pts.  acetone 
at  10°. 


(Laszczynski,  B.  1894,  27.  2286.) 


Solubility   in    ethyl   acetate- 1  : 3.466   at 
18°.    (Alexander,  Dissert.  1899.) 


Solubility  of  HgCl2  in  ethyl  acetate. 


Temp. 

0° 

13° 

30° 

40.5° 

50.2° 

Mol.  HgCl2  in  100 
mols.  C4H8O2 

15.4 

15.9 

16.0 

16.1 

16.3 

(Linebarger,  Am.  Ch.  J.  1894,  16.  214.) 

1  g.  HgCl2  is  sol.  in  3.5  g.  ethyl  acetate  at 
18°.  Sp.  gr.  of  sat.  solution  18°/4°  =  1.110. 
(Naumann,  B.  1904,  37.  3602.) 


504 


MERCURIC  CHLORIDE 


Solubility   of   HgCl2   in   ethyl 

acetate   and 

Sat.  solution 

acetone  at  t°. 

Solvent 

t 

contains 

%  HgCl2 

t° 

Molecules 
HgCU  sol. 
in  100  mol- 
ecules of 
ethyl 

Molecules 
HgClz  sol. 
in  100  mol- 
ecules of 
acetone 

Solid  present  in 
acetone 

Ethyl  alcohol 

—60 
—55 
—43 
—40 

3.0 

7.8 
8.8 
9.8 

acetate 

—30 

14.3 

—15 

9.10 

14.5     HgCl2,  CH3COCH3 

—23 
21 

18.6 

1Q     1 

0 

9.25 

14.3 

'• 

—20 

J-t7  .   X 

21.9 

+10 
10 

.... 

18.7 
23.5 

HgCl, 

—17 
—11 

22.1 
24.7 

17 

.... 

23.2 

,  g 

27  0 

25 

9.15 

22.8 

u 

—  5 

29^7 

(Aten,  Z.  phys.  Ch.  1906,  54.  121.)      . 

0 
+  3 

29.0 
30.0 

7 

30.9 

Solubility  of  HgCl2 

in  ethyl 

c\  pro 

acetate  +Aq  at 

10 
14 

31.3 
31.3 

&V    . 

19 

32.0 

P  =  g.  ethyl  acetate  in  100 

g. 

ethyl  acetate 

31 

34.2 

+Aq. 

43 

36.4 

HgCl2  =millimols 

.  HgCl2  in 

10  cc.  of  the 

51 

38.9 

solution. 

62 

42.1 

63 

42  5 

P 

HgCU 

Sp.  gr. 

68 

44^7 

A  CT     O 

0 

2.67 

1.0565 

80 

45.2 

48.0 

4 

.39 

2.72 

1.0581 

92 

51.0 

96.76 

15.34 

1.2371 

93 

51.4 

100 

9.75 

1.1126 

100. 

1  -1  K 

53.6 

ftfk    A 

(Herz  and  Anders, 

Z.  anorg. 

1907,  52.  172.) 

110 

127 

OU.O 

65.3 

138               67.8 

1  pt.  is  sol.  in  2.05  pts.  ethyl  acetate  at  18° 
or  100  g.  ethyl  acetate  dissolve  48.7  g.  HgCl2. 
(Naumann,  B.  1910,  43.  315.) 

N-propyl  alcohol 

—32 
—22 
—14 
0 

14.7 
15.4 
15.6 
16.4 

Easily  sol.  in  glycerine;   sol.   in   14   pts. 
glycerine.     (Fairley,   Monit.   Scient.    (3)   9. 

0 
+16 
41 

16.5 
18.2 
23.8 

685.) 

53 

27  9 

100  g.  glycerine  dissolve  80  g.  HgCl2  at  25°. 
(Moles  and  Maquina,  Ann.  Soc.  Eshan.  fis 

62 
67 

29^4 
32.7 

quin. 

1914,  12. 

383.) 

78 

36.4 

100 

43.8 

Solubility  in  organic 

solvents 

127 

52.7 

Allyl  alcohol 

-21 

9O   fi 

Solvent 

t° 

Sat.  solution 

—  1 

+J\J  .  \J 

29.6 

contains 

1        0 

9J  HgCb 

-[-     O 

oo  .  £ 

22 

48.7 

Methyl  alcohol 

—34 

7.6 

Acetone 

—23 

51.4 

—20 

11.5 

—18 

52.9 

—15 

12.8 

—15 

56.6 

—  2 

18.7 

—10 

56.7 

+  4 

23.2 

—  8 

58.4 

12 

27.6 

—  4 

59.1 

36 

53.1 

—  1 

60.1 

51 

61.0 

+  6 

61.9 

62 

63.6 

12 

61.4 

64 

63.7 

15 

61.8 

74 

64.3 

27 

62.0 

100 

68.7 

36 

61.9 

127 

75.2 

54 

62.1 

MERCURIC  CHLORIDE 


505 


Solubility  in  organic  solvents.  —  Continued. 

Solubility  in  organic  solvents.  —  -Continued. 

Solvent 

t° 

Sat.  solution 
contains 
%  HgCU 

Solvent 

t° 

Sat.  solution 
contains 
%  HgCh 

N-butyl  alcohol 

—21 
—  6 
+  9 
21 
59 
82 

12.4 
13.0 
14.3 
15.9 

25.8 
33.1 

Acetic  acid 

+21 
22 
33 
43 
50 
61 
87 
95 
95 
115 
116 
127 
145 
182 
207 

2.7 
3.0 
5.0 
6.0 
6.7 
8.0 
11.0 
12.0 
12.5 
16.0 
17.0 
20.0 
26.3 
44.8 
55.2 

Isobutyl  alcohol 

—11 
—  6 
0 
+11 
63 
98 
127 
145 
155 

5.5 
6.2 
6.7 
7.5 
19.3 
32.1 
42.0 
47.2 
50.4 

Amyl  alcohol 

13 

8.6 
8.9 
14.0 
29.8 
35.1 

+26 
50 
90 
106 

Formic  acid 

21 
50 
90 

2.0 
3.2 
7.3 

Very  si.  sol.  in  propionic  and  isobutyric 
acids. 

(Etaid,  A.  ch.  1894,  (7)  2.  557  et  seq.) 
Solubility  of  HgCl2  in  organic  solvents  at  t°. 

Ether 

—47 
—40 
—35 
—30 
—19 
0 
+13 
83 
100 
115 

5.6 

5.8 
6.1 
5.9 
5.6 

5.8 
5.8 
8.4 
8.7 
9.0 

Solvent 

t 

%  HgCI2 

Ethyl  formate 

—20 
—  3 

+24 
+46 

29.6 
29.2 
30.0 
31.0 

CHC13 

—20.5 

+44.2 

0.01 
0.12 

C6H6 

+6.5 
18.0 
34.1 
54.1 
69.0 

0.26 
0.53 
0.64 
1.02 
1.39 

Ethyl  acetate 

—50 
—20 
—14 
—  6 
0 
+  7 
19 
45 
66 
100 
131 
150 
180 

39.6 
40.5 
40.2 
40.0 
39.5 
39.9 
40.2 
41.6 
44.0 
47.8 
50.1 
57.0 
59.3 

C2H4C12 

0 
12.5 
20.8 
25.3 
30.2 
33.0 
45.9 

1.33 
1.55 
1.68 
1.73 
1.92 
2.05 
2.42 

Methyl  acetate 

—20 
+24 
55 

42.0 
40.3 
41.5 

CH3COOC2H5 

0 
6.5 
26.1 
38.5 
45.3 

22.8 
22.7 
22.8 
23.5 
26.4 

Amyl  acetate 

+22 
48 

18.3 
18.5 

Ethyl  butyrate 

+20 
55 
71 

12.6 
13.5 
15.1 

Dukelski,  Z.  anorg.  1907,  63.  329. 

506 


MERCURIC  CHLORIDE 


Solubility  of  HgCl2  in  mixed  organic  solvents 
at  t°. 

Solubility  of  HgCl2  in  mixed  organic  solvents 
at  t°  —  Continued. 

Solvent 

t° 

%  HgCl2 

Solvent 

t 

HgCh 

C6H6+C2H5OH 

—2.5 
0.0 
6.0 
20.5 
20.65 
24.5 
34.5 
54.4 
54.5 

15.20 
15.40 
16.38 
18.40 
18.50 
19.33 
21.34 
24.84 
24.42 

C2H4C12+CH3OH 

0.0 
12.5 
20.8 
25.3 
30.2 
33,0 

37.4 
45.9 

13.33 
21.30 
29.23 
34.78 
36.87 
37.01 
37.95 
39.36 

CH3COOC2H6+C6H6 

0.0 
6.5 
'25.7 
27.6 
35.5 
45.3 

9.62 
9.62 
9.78 
9.78 
10.81 
13.69 

C6H6+2C6H5OH 

—5.2 
0 

+9.1 
20.9 
24.4 
36.5 
53.7 
74.0 

19.45 
20.13 
21.65 
23.57 
24.19 
26.53 
31.27 
38.74 

CH3COOC2H6+CHC13 

0.0 
26.1 
36.1 
46.0 
48.5 

3.34 
4.07 

4.78 
5.38 
5.10 

CHC13+C2H6OH 

—20.5 
—12.0 
0.0 
+8.0 
23.0 
38.5 
44.2 
45.6 

3.82 
4.43 
4.89 
5.37 
7.12 
8.51 
9.51 
9.98 

2CH3COOC2H6+CC14 

0.0 
10.3 
25.7 
27.6 
38.5 
45.3 

9.24 
9.05 
9.32 
9.50 
9.89 
11.70 

CHC13+2C2H6OH 

—20.5 
0.0 

+8.0 
23.0 
38.5 
44.2 

6.60 
7.69 
8.96 
10.66 
12.50 
14.40 

(Dukelski,  Z.  anorg.  1907,  63.  335.) 

Solubility  in  organic  solvents  at  18°/20°. 
100  g.  chloroform  dissolve  0.106  g.  HgCl2. 
100  g.  tetrachlormethane  dissolve  0.002  g. 
HgCl2. 
100  g.  bromoform  dissolve  0.486  g.  HgCl2. 
100   g.    ethyl   bromide   dissolve   2.010   g. 
HgCl2. 
100  g.  ethvlene  dibromide  dissolve  1.530  g. 
HgCl2.    (Silk  Z.  anorg.  1900,  25.  401.) 

Solubility  of  HgCl2  in  various  organic 
solvents  at  25°. 
G.  =g.  HgCl2  dissolved  in  1  mol.  of  solvent. 

CHC13+CH3OH 

—12.0 
0.0 
+8.0 
23.0 
24.9 
30.6 
38.5 

1.73 
3.51 
5.63 
10.15 
10.71 
11.40 
12.02 

CHC13+2CH3OH 

—12.0 
0.0 
+8.0 
23.0 
24.9 
30.6 
38.5 

3.33 
6.73 
8.21 
16.56 
18.45 
19.70 
20.83 

Solvent                                   G.  HgCl2 

Ethylene  chloride                      1  .  216 
Tetrachlorethane                       0.146 
Chloroform                                 0.120 
Dichlorethylene                    ,     0.110 
Pentachlorethylene                   0  .  039 
Trichlorethylene                        0  .  036 
Perchlorethylene                        0  .  012 
Carbon  tetrachloride                 Trace 

CC14+2CH3OH 

0.0 

7.7 
24.9 
30.6 
35.5 
36.1 
48.5 

'5.20 
6.69 
14.06 
19.40 
20.50 
21.80 
21.90 

(Hofman,  et  al.,  B.  1910,  43.  188.) 

Very  si.  sol.  in  nitromethane  at  ord.  temp. 
Very  sol.  on  warming.    (Bruner,  B.  1903,  36. 
3298.) 

MERCURIC  HYDROGEN  CHLORIDE 


£07 


Solubility  in  CS2  at  t°. 

Solubility  of  HgCl2  in  pyridine.  —  Continued. 
t  =  point  of  fusion. 
Solid  Phase  =  HgCl2,  C8H5N. 

.    t° 

100  pts.  sat.  solution 
contain  pts.  HgCh 

—10 
—  5 
0 
+  5 
10 
15 
20 
25 
30 

0.010 
0.014 
0.018 
0.022 
0.026 
0.032 
0.042 
0.053 
0.063 

t° 

HgCl2 

t° 

% 

HgCl2 

t° 

H?C1 

74.7 
83.5 
86.5 
87.3 

48.38 
50.53 
52.37 
52.02 

90.61 
75.0° 
99.5 
99.5 
100.5 

53.50 
56.45 
56.07 
57.01 

57.84 

104.1 
104.2 
104.7 
107. 

60.09 
60.72 
58.97 
63.06 

Solid  Phase  =  3HgCl2,  C6H5N. 

(Arctowski,  Z.  anorg.  1894,  6.  267.) 

0.030  g.  is  dissolved  in  100  g.  sat.  solution 
in  CS2  at  8°.    (Arctowski,  Z.  anorg,  1894,  6. 
256.) 
Formic  acid  (95%)  dissolves  2.1%  at  19°. 
(Aschan,  Ch.  Z.  1913,  37.  1117.) 
Sol.    in    molten    urethane.      (Castoro,    Z. 
anorg.  1899,  20.  61.) 
Sol.  in  ethyl  sulphocyanate.    (Kahlenberg, 
Z.  phys.  Ch.  1903,  46.  66.) 

t° 

A, 

t° 

HgCl2 

t 

H&l, 

94.7 
95.2 
106.4 
109.8 

60.72 
60.77 
61.93 

62.58 

113.6 
114.0 
115.7 
118.2 

63.06 
63.18 
63.37 
64.09 

124.2 
129.4 
145.5 

65.00 
65.63 
69.66 

(McBride,  Z.  phys.  Ch.  1910,  14.  196.) 

Solubility  in  pyridine. 
S  =  temp.  of  solidification. 

Solubility  of  HgCl2  in  benzene. 
100  pts.  C6H6  dissolve  at: — 
15°      41°      55°      84° 
0.54     0.62    0.85     1.80  pts.  HgCl2. 

(Laszcynski,  B.  1894,  27.  2287.) 


Solubility  in  C6H6  =  0.0197  mol./l.  at  25°. 
(Sherrill,  Z.  phys.  Ch.  1903,  43.  735.) 

Sol.  in  C6H6,  toluene,  xylene,  and  other  aro- 
matic hydrocarbons.  Insol.  or  only  si.  sol. 
in  petroleum  ether,  hexane,  decane  and  CS2. 
(Gulewitsch,  B.  1904,  37.  1563.) 

Sol.  in  p-toluidine.    (Werner.) 

Sol.  in  quinoline.  (Beckmann  and  Gabel, 
Z.  anorg.  1906,  51.  236.) 


Solubility  of  HgCl2  in  pyridine. 
= point  of  fusion. 

Solid  Phase  =  HgCl2,  2C5H6N. 


t° 

% 

HgCl2 

t 

% 

HgCl2 

t° 

A, 

—32.8 

2.76 

40.90 

29.29 

78.0 

49.72 

—21.9 

7.86 

5C.10 

34.94 

78.7 

50.37 

+  0.02 

13.14 

60.03 

40.36 

80.2 

51.52 

12.58 

17.34 

7C.15 

46.44 

82.5 

52.40 

18.78 

19.78 

70.8 

45.77 

89.0 

56.45 

23.60 

21.59 

74.6 

48.00 

90.8 

57.01 

27.23 

22.65 

75.2 

48.38 

94.1 

60.09 

31.05 

24.46 

76.4 

49.15 

Mols. 
per  100 

s 

Mols. 
per  100 

.     s 

Mols. 
per  100 

s 

5.8 

19 

27.0 

87 

38.5 

130 

5.9 

18.5 

28.6 

(98) 

41.0 

137 

10.2 

39.5 

30.3 

91.5 

43.2 

142 

14.1 

52 

31.2 

92 

44.0 

143.5 

21.4 

74.5 

33.1 

108 

47.5 

159 

25.0 

83 

35.1 

115.5 

52.8 

173 

(Staronka,   Anz.   Ak.   Wiss.   Krakau,    1910. 

372.) 

Sp.  gr.  at  16°/4°  of  HgCl2+pyridine  contain- 
ing 17.53%  HgCl2  =  1.1523;  containing  6.57% 
HgCl2  =  1.0388.  (Schonrock,  Z.  phys.  Ch 
1893,  11.  768.) 

Mol.  weight  determined  in  benzonitrile, 
methyl-  and  ethyl-sulphide.  (Werner,  Z. 
anorg.  1897,  15.  31.  26  and  30.) 

Sol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1369.) 

Easily  sol.  in  oil  of  turpentine  and  other 
essential  oils;  si.  sol.  in  cold  benzene,  but 
much  more  on  heating,  crystallising  on  cool- 
ing. (Franchimont,  B.  16.  387.) 

Easily  sol.  in  boiling  creosote. 

Insol.  in  olive  oil. 

Insol.  in  oils  and  fats  but  sol.  when  first 
dissolved  in  alcohol,  free  ether  or  anhydrous 
ketones.  (Glock,  Ch.  Z.  Repert.  36.  315.) 

Extracted  from  HgCl2+Aq  by  volatile  oils. 

Mercuric  hydrogen  chloride  (Chloromercuric 
acid),  HgCl2,  HCl  =  HHgCl3. 

Decomp.  by  H2O,  (Boullay,  A.  ch.  34. 
24o.) 

Easily  decomposed.  (Neumann,  M.  10. 
236.) 


508 


MERCURIC  HYDRAZINE  CHLORIDE 


HgCJ2,  2HC1+7H2O.     Decomp.  by  H2O. 
(Ditte,  A.  ch.  (5)  22.  551.) 
3HgCl2,  4HC1+14H20.    As  above. 
2HgCl2,  HC1+6H2O.    As  above. 
4HgCl2,  2HC1+9H2O.    As  above. 
3HgCl2,  HCl-f  5H2O.    As  above. 

Mercuric  hydrazine  chloride,  HgCl2, 

2(N2H4,  HC1). 

Very  sol.  in  H2O.  More  sol.  in  hot  alcohol 
than  in  cold;  decomp.  by  HNO3.  (Curtius, 
J,  pr.  1894,  (2)  50.  332.) 

Mercuric    nickel    chloride,    basic,     HgCl2, 
6NiO,  NiCl2+20H2O,  and  HgCl2,  7NiO, 
NiCl2. 
(Mailhe,  A.  ch.  1902,  (7)  27.  369.) 

Mercuric  nickel  chloride. 

Deliquescent,    (v.  Bonsdorff.) 

Mercuric  nitrosyl  chloride,  HgCl2,  NOC1. 

Sol.  in  H2O  without  effervescence.  (Sud- 
borough,  Chem.  Soc.  59.  659.) 

Mercuric  phosphoric  chloride,  3HgCl2,  2PC15. 
Decomp.  and  dissolved  by  H2O.    (Baudri- 
mont,  A.  ch.  (4)  2.  45.) 

Mercuric  potassium  chloride,  2HgCl2,  KC1+ 
2H2O. 

Very  easily  sol.  in  warm  H2O.  A  clear 
solution  at  18°  is  filled  with  crystals  at  15°. 
SI.  sol.  in  alcohol,  (v.  Bonsdorff,  Pogg.  17. 
122.) 

HgCl2,  KC1+H2O.  Easily  sol.  in  H2O;  si. 
sol.  in  alcohol,  (v.  Bonsdorff,  Pogg.  19.  336.) 

HgCl2,  2KC1+H2O.    As  above. 

Solubility  determinations  show  that  the 
double  salts  formed  by  mercuric  and  potas- 
sium chlorides  at  25°  are: 

2KC1,  HgCl2+H20. 

KC1,  HgCl2+H2O.  Can  be  recryst.  with- 
out decomp. 

KC1,  2HgCl2+2H2O.  Gives  HgCl2  on 
recryst.  from  H2O.  (Foote  and  Levy,  Am. 
Ch.  J.  1906,  35.  237.) 

Mercurous  rhodium  chloride. 

See  Chlororhodite,  mercurous. 
Mercuric  rubidium  chloride,  HgCl2,  RbCl. 

Sol.  in  H2O. 

HgCl2,  2RbCl.  Sol.  in  H2O  and  HCl+Aq. 
(Godeffroy,  Arch.  Pharm.  (3)  12.  47.) 

+2H2O.    Sol.  inH2O.    (Godeffroy.) 

2HgCl2,  RbCl.    Sol.  in  H2O.    (Godeffroy.) 

Solubility  determinations  show  that  at  25° 
there  exist  five  double  mercuric  rubidium 
chlorides  with  the  following  formulas: 

RbCl,  5HgCl2.  Gives  HgCl2  on  recryst. 
from  H2O. 

3RbCl,4HgCl2+H2O.    Gives  RbCl, 
5HgCl2  on  recryst  from  H2O. 

RbCl,  HgCl2+H2O.  Gives  3RbCl,  4HgCl2 
on  recryst.  from  H2O. 


3RbCl,  2HgCl2+2H2O.  Gives  3RbCl, 
4HgCl2  on  recryst.  from  H2O. 

2RbCl,  HgCl2+H2O.    Gives  3RbCl, 
4HgCl2  on  recryst  from  H2O. 

(Foote  and  Levy,  Am.  Ch.  J.  1906,  35.  241.) 

Mercurous  silver  chloride,  HgCl,  AgCl. 
(Jones,  J.  Soc.  Chem.  Ind.  1893,  12.  983.) 
2HgCl,   AgCl.     Min.  Bardosite.      (Jones, 

J.  Soc.  Chem.  Ind.  1893,  12.  983.) 

3HgCl,  AgCl.     (Jones,  Chem.  Soc.  1910, 

97.  338.) 

Mercuric  sodium  chloride,  HgCl2,  NaCl. 

Sp.  gr.  at  16°/4°  of  aqueous  solution  con- 
taining 14.937%  salt  =  1.13310;  containing 
11.0736%  =  1.09528.  (Schonroek,  Z.  phys. 
Ch.  1893,  11.  782.) 

+H2O.  (Linebarger,  Am.  Ch.  J.  1893,  16. 
344.) 

+1^H20.  Sol.  in  0.33  pt.  H2O  at  15°. 
(Schindler,  Repert.  36.  240.) 

Extremely  easily  sol.  in  alcohol.    (Voit.) 

Sol.  in  275  pts.  ether.  Ether  dissolves  the 
undecomposed  salt  out  of  H2O  solution. 
(Lassaigne,  A.  ch.  64.  104.) 

HgCl2,  2NaCl.  Deliquescent.  Very  sol. 
in  H2O.  (Voit,  A.  104.  354.) 

2HgCl2,  NaCl.  Decomp.  by  H2O  in  dil. 
solution.  Sol.  in  acetone  and  acetic  ether. 
(Linebarger,  Am.  Ch.  J.  1893,  15.  344.) 

Solubility  determinations  show  that  the 
only  double  salt  formed  by  mercuric  and 
sodium  chlorides  between  10.3°  and  25°  is 
NaCl,  HgCl2+2H2O.  Can  be  recryst.  from 
H2O.  (Foote  and  Levy,  Am.  Ch.  J.  1906,  35. 
237.) 

Mercuric   strontium  chloride,   basic,   SrCl2, 

HgO+6H20. 
Decomp.  by  H2O.    (Andre,  C.  R.  104.  431.) 

Mercuric  strontium  chloride,  2HgCl2,  SrCl2  + 

2H2O. 

Easily  sol.  in  H2O.    (v.  Bonsdorff.) 
3HgCl2,    SrCl2+5-6H2O.      Very    sol.    in 

H2O.    (Swan,  Am.  Ch.  J.  1898,  20.  632.) 

Mercurous  sulphur  chloride. 
See  Mercurous  sulphochloride. 

Mercuric  thallous  chloride,  HgCl2,  T1C1. 

Easily  sol.  in  H2O.  (Jorgensen,  J.  pr.  (2) 
6.  83.) 

Mercurous  stannous  chloride,  Hg2Cl2,  SnCl2. 
Decomp.  by  H2O.     (Capitaine.  J.  Pharm. 
25.  549.) 

Mercuric  yttrium  chloride,  3HgCl2,  YC13  + 
9H2O. 

Deliquescent.  Verv  sol.  in  H2O.  (Popp, 
A.  131.  179.) 


MERCUROUS  IODIDE 


509 


Mercuric  zinc  chloride,  HgCl2,  ZnCl2. 

Very  sol.  in  H2O.    (Harth,  Z.  anorg.  1897, 
14.  323.) 

2HgCl2,  ZnCl2.     (Varet,  C.  R.  1896,  123. 

422.) 

Mercuric    zinc    chloride    ammonia,    HgCl2, 

4ZnCl2,  10NH3+2H2O. 
•    Insol.  in  boiling  H2O,  but  decomp.  thereby. 
(Andre,  C.  R.  112.  995.) 

HgCl2,  2ZnCl2,  6NH3  +  ^H2O.    As  above. 
(Andre.) 

Mercuric  chloride  ammonia,  HgCl2,  12NH3. 
SI.  sol.  in  ammonia.     (Franklin,  Am.  Ch. 
J.  1900,  23.  300.) 

Mercuric  chloride   cadmium   oxide,   HgCl2, 

CdO+H2O. 
(Mailhe,  A.  ch.  1902,  (7)  27.  371.) 

Mercuric  chloride  cobaltous  oxide,   HgCl2, 


(Mailhe,  C.  R.  1901,  132.  1274.) 

Mercuric  chloride  cupric  oxide,  HgCl2,  3CuO 

+H20. 
(Mailhe,  Bull.  Soc.  1901,  (3)  25.  791.) 

Mercuric  chloride  hydrazine,  HgCl2,  N2H4. 

Very  unstable.  Decomp.  by  H2O.  Pptd. 
from  alcohol  solution  by  H2O;  very  sol.  in 
min.  acids  with  decomp. 

Easily  sol.  in  HC1  or  HNO8.  Decomp.  by 
alkalies.  Somewhat  sol.  in  acetic  acid.  (Hof- 
mann,  B.  1897,  30.  2020.) 

Mercuric    chloride    hydroxylamine,    HgCl2, 

2NH2OH. 

Completely  sol.  in  methyl  and  ethyl  al- 
cohol; insol.  in  ether:  decomp.  by  H2O  and 
NaOH+Aq.  Sol.  in  NH2OH,HCl+Aq. 
(Adams,  Am.  Ch.  J.  1902,  28.  210.) 

Mercuric  chloride  lead  oxide,  HgCl2,  2PbO  + 

2H20. 
(Mailhe,  A.  ch.  1902,  (7)  27.  372.) 

Mercuric  chloride  strontium  chromate, 

2HgCl2,  HC1,  SrCrO4. 
Sol.  in  H2O  without  decomp.      (Imbert, 
Bull.  Soc.  1897,  (3)  17.  471.) 

Mercuric  chloroiodide,  2HgCl2,  HgI2. 

Sol.  in  H2O.    (Liebig.) 

HgCl2,  HgI2.  SI.  sol.  in  hot  H2O  with 
partial  decomp.  More  easily  sol.  in  alcohol. 
(Kohler,  B.  12.  1187.) 

Mercurous  fluoride,  Hg2F2. 
Decomp.  by  H2O  with  separation  of  Hg2O. 

Mercuric  fluoride,  HgF2+2H2O. 

Decomp.  by  cold  H2O,  with  separation  of 
HgO.  Sol.  in  dil.  HNO3+Aq,  and  HF+Aq. 
(Finkener,  Pogg.  110.  628.) 


Mercurous  hydrogen  fluoride,  Hg2F2,  4HF  + 

4H20. 

Deliquescent.  Easily  sol.  in  H2O.  Sol.  in 
dil.  acids  and  dil.  HF.  (Bohm,  Z.  anorg. 
1905,  43.  327.) 

Mercurous  silicon  fluoride. 
See  Fluosilicate,  mercurous. 

Mercurous  fluoride  ammonia,  Hg2F2,  2NH3. 
Stable  on  air.    (Finkener,  Pogg.  110.  142.) 

Mercurous  hydroxide,  HgOH. 

Nearly  insol.  in  cold,  sol.  in  hot  H2O. 
Sol.  in  NaOH+Aq.  (Bhaduri,  Z.  anorg. 

1897,  13.  410.) 

Mercurous  iodamide,  Hg2(NH2)I. 

(Rammelsberg,  Pogg.  48.  184.) 

Is  a  mixture  of  Hg  and  Hg(NH2)l.  (Bar- 
foed.) 

Mercurous  iodide,  Hg2I2. 

Sol.  in  over  2375  pts.  H2O.  (Saladin,.J. 
chim.  med.  7.  530.) 

Solubility  in  H2O  =  2.6x  10  8  g.-equiv.  per 
liter  (calculated).  (Bodlander,  Z.  phys.  Ch. 

1898,  27.  58.) 

Solubility  in  H2O  =  3  x  10 -10  mols.  per  litre 
at  25°.  (Sherrill,  Z.  phys.  Ch.  1903,  43.  735.) 

Sol.  in  Hg(NO3)2+Aq.  (Stromann,  B.  20. 
2815.) 

Sol.  in  KI+Aq.  Easily  sol.  in  Hg2(NO3)2  + 
Aq.  SI.  sol.  in  NH4OH+Aq.  Sol.  in  hot 
NH4Cl+Aq,  but  less  than  HgI2.  Less  sol. 
in  NH4NO3  than  in  NH4Cl+Aq.  (Brett.) 

Partially  sol.  with  separation  of  Hg  and 
formation  of  HgI2,  in  cold  KI+Aq,  hot  Nal, 
CaI2,  SrI2,  BaI2,  MgI2,  ZnI2,  and  NH4I+Aq; 
in  warm  NaCl,  KC1  and  NH4Cl+Aq,  and 
slowly  in  hot  HCl+Aq.  (Boullay,  A.  ch.  (2) 
34.  358.) 

Decomp.  by  alkali  chlorides +Aq.  (Miahle, 
A.  ch.  (3)  6.  177.) 

Very  easily  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  829.) 

Not  wholly  insol.  in  alcohol,  ether,  or  chlor- 
oform. (Maclagan,  Rep.  anal.  Ch.  1884.  378.) 

Decomp.  by  boiling  alcohol:  1000  g.  boiling 
alcohol  decomp.  about  3.15  g.  Hg2I2.  (Fran- 
gois,  C.  R.  1896,  121.  890.) 

Boiling  alcohol  decomp.  Hg2I2  to  Hg  and 
HgI2  which  dissolves  until  0.220  g.  HgI2  are 
contained  in  100  g.  alcohol.  (Frangois,  C.  R. 

1896,  121.  889.) 

Insol.  in  cold  ether.     (Frangois,  J.  Pharm. 

1897,  (6),  6.  445.) 

Insol.  in  methylene  iodide.  (Retgers,  Z. 
anorg.  3.  345.) 

Difficultly  sol.  in  methyl  acetate.  (Nau- 
mann,  B.  1909,  42.  3790.) 

Phenol  at  180°  decomp.  it  into  Hg  and  HgI2 
until  a  state  of  equilibrium  is  reached  with 


510 


MERCURIC  IODIDE 


2.75  g.  HgI2  to  100  g.  phenol,  above  which 
point  Hgl  is  si.  sol.  (0.05  g.  in  100  g.)  in 
phenol-HgI2  mixture.  Decomp.  by  cold 
aniline  more  rapidly  than  by  hot.  Equil- 
ibrium is  reached  when  26.35  g.  HgI2  are 
present  to  100  g.  aniline  at  bpt.  of  aniline. 
Aniline  containing  more  than  26  g.  HgI2  to 
100  g.  dissolves  Hgl  in  considerable  quan- 
tity. (Francois,  C.  C.  1896,  I,  470.) 

SI.  sol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1369.) 

SI.  sol.  in  allyl  mustard  oil.  (Mathews,  J. 
phys.  Chem.  1905,  9.  647.) 

Mercuric  iodide,  HgI2. 

Sol.  in  150  (?)  pts.  H2O.      (Wiirtz.) 

1  1.  H2O  at  17.5°  dissolves  0.0403  g.  HgI2. 
(Bourgpin,  A.  ch.  (6)  3.  429.) 

Sol.  in  about  6500  pts.  H2O.    (Hager.) 

According  to  calculation  from  electrical 
conductivity  of  HgI2+Aq,  HgI2  is  much  less 
sol.,  1  1.  H2O  dissolving  only  0.5  mg.  HgI2  at 
18°.  (Kohlrausch  and  Rose,  Z.  phys.  Ch.  12. 
241.) 

1  1.  H2O  dissolves  0.054  g.  HgI2  at  22°. 
(Rohland,  Z.  anorg.  1898,  15.  412.) 

1  1.  H2O  at  25°  dissolves  about  0.06  g. 
(Morse,  Z.  phys.  Ch.  1902,  41.  731.) 

1  1.  H2O  at  18°  dissolves  4x10^  mol. 
(Abegg,  Z.  Elektrochem.  1903,  9.  553.) 

Solubility  in  H2O  at  25°  =  0.00013  mol. 
liter.  (Sherrill,.Z.  phys.  Ch.  1903,  43.  735.) 

1  1.  H2O  dissolves  0.4  mg.  HgI2  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1904,  50.  356.) 

1  1.  H2O  at  18°  dissolves  0.2  to  0.4  mg. 
(Kohlrausch,  Z.  phys.  Ch.  1908,  64.  168.) 

The  yellow  modification  is  always  deposited 
from  solution  even  in  the  presence  of  an  ex- 
cess of  the  red  form.  (Gernez,  C.  R.  1903, 
136.  1323.) 

Sol.  in  many  acids,  especially  in  HC1,  and 
HI+Aq.  Insol.  in  HC2H302+Aq.  (Berthe- 
mot.)  Scarcely  sol.  in  dil.  HNO3+Aq. 

Not  attacked  by  cold  H2SO4,  decomp.  by 
hot.  (Ditte,  A.  ch.  1879,  (5)  17.  124.) 

Sat.  solution  in  H2SO3+Aq  contains  at 
critical  temp.  (158.2°),  0.7%  HgI2.  (Niggli, 
Z.  anorg.  1912,  75.  182.) 

Sol.  in  hot  (NH4)2CO3,  (NH4)2SO4,  cold 
NH4C1,  NH4NO3,  or  ammonium  succinate+ 
Aq.  (Wittstein.) 

Sol.  in  HgCl2,  Hg(N03)2,  or  Hg(C2H3O2)2  + 
Aq.  Easily  sol.  in  Na2S2O3+Aq.  Easily  sol. 
in  soluble  iodides +Aq.  More  sol.  in  hot  than 
in  cold  Nal  or  KI+Aq.  When  cone.,  1  mol. 
KI  in  hot  solution  dissolves  3  mols.  HgI2,  but 
a  portion  separates  on  cooling:  BaI2,  SrI2, 
MgI2,  and  CaI2  act  in  the  same  way.  Easily 
sol.  in  cold,  more  sol.  in  hot  ZnI2+Aq,  2  mols. 
HgI2  beipg  dissolved  to  1  mol.  ZnI2.  In  NHJ 
+Aq,  3  mols.  HgI2  are  dissolved  to  2  mols. 
NHJ.  Abundantly  sol.  in  hot  KC1,  NaCl, 
NH4Cl+Aq,  but  separates  out  on  cooling,  and 
the  trace  remaining  may  be  pptd.  by  H2O, 
2  g.  KC1  in  solution  dissolves  1.166  g.  HgI2. 
Sol.  in  HgCl2+Aq,  and  very  easily  sol.  in 


alcoholic  solution  of  HgCl2.    (Boullay,  A.  ch. 
(2)  34.  346.) 

Solubility  in  MI+Aq  at  25°. 


Salt 

In  10  ccm.  of  the  solution 

Millimols  HgI2 

Millimols  salt 

Nal 

4.12 
6.22 
9.45 

7.94 
13.85 
22.25 

KI 

1.27 
1.80 
5.10 
7.00 
12.24 

3.03 
3.90 
10.34 
15.54 
25.19 

CaI2 

0.50 
2.61 
4.40 
4.58 
17.06 

0.53 
2.52 

4.68 
4.84 
17.99 

SrI2 

2.12 
3.20 

5.82 
6.94 

2.54 
3.55 
5.39 
6.08 

BaI2 

0.59 

7.42 
8.98 
14.62 

0.99 

7.48 
9.78 
15.08 

(Herz  and  Paul,  Z.  anorg.  1913,  82.  434.) 
Solubility  of  HgI2+KI  in  H20. 

Temp  =20°. 

%KI 

%  Hgl  2 

Solid  phase 

50.9 
44.4 
39 
37.4 
37.8 
35.1 
35.5 
26.7 
26.6 
23.7 
14.9 

19.3 
32.4 
48 
53.6 
52.6 
52.2 
51.2 
50.3 
49.4     . 
40.2 
22.5 

KI 

KI+KHgI3 
KHgI3 

1C 

KHgI3,  H2O 
KHgI3+HgI2 
HgI2 

u 

Temp.  =30° 

60.6 
40 
39.6 
40 
40.2 
39.3 
33.7 
33 
31.4 
29.1 

53 
52.7 
52.2 
51.2 
50.3 
49.8 
52 
51.7 
52.2 

KI 
KI-fKHgI3 
KHgI3 

KHgI3,  H20 

(Dunningham,  Chem.  Soc.  1914,  105.  368.) 

MERCURIC  IODIDE 


511 


Very  sol.  in  KSCN+Aq.  (Philipp,  Pogg. 
1867,  131.  93.) 

Sol.  in  1.09  pts.  cryst.  Na2S2O3+Aq. 
(Eder  and  Uhn,  M.  1882,' 3.  197.) 

Very  sol.  in  hot  CaCl2+Aq,  less  sol.  in 
BaCl2,  KC1  and  NaCl+Aq.  (Lea,  Z.  anorg. 
1896,  12.  341.) 

Solubility  in  normal  Hg(NO3)2+Aq  = 
48.0  g.  per  litre.  (Morse,  Z.  phys.  Ch.  1902, 
41.  731.) 

Extremely  sol.  in  cold  cone.  NH4Br+Aq. 
(Grossmann,  B.  1903,  36.  1602.) 

Sol.  in  alkali  sulphites +Aq.  (Barth,  Z. 
phys.  Ch.  1892,  9.  215.) 

Sol.  in  Ca(OCl)2+Aq;  sol.  in  KOH+Aq. 
(Melsens,  A.  ch.  (3)  26.  222.) 

Sol.  in  liquid  SO2.  (Walden  and  Cent- 
nerszwer,  C.  C.  1992,  I.  344.) 

Very  easily  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  829.) 

Sol.  in  SOC12,  S2C12,  SO2C12,  warm  AsCl3, 
PBr3,  warm  POC13.  (Walden,  Z.  anorg. 
1900,  25.  212.) 

Easily  sol.  in  AsBr3.  (Walden,  Z.  anorg. 
1902,  29.  374.) 

Insol.  in  liquid  CO2.  (Buchner,  Z.  phys. 
Ch.  1906,  64.  674.) 

More  sol.  in  alcohol  than  in  H2O.  1  1. 
H2O  containing  10%  of  90%  alcohol  dis- 
solves 0.08  g.  HgI2.  1  1.  of  alcohol  of  80°  B. 
dissolves  2.851  g.  HgI2,  1  1.  absolute  alcohol 
dissolves  11.86  g.  HgI2.  (Bourgoin,  A.  ch. 
(6)  3.  429.) 

Sol.  in  130  pts.  cold,  and  15  pts.  hot  90% 
alcohol.  (Hager.) 

100  pts.  absolute  methyl  alcohol  dissolve 
3.16  pts.  at  19.5°;  100  pts.  absolute  ethyl 
alcohol  dissolve  2.09  pts.  at  19.5°.  (de 
Bruyn,  Z.  phys.  Ch.  10.  783.) 

0.00842  pt.  is  sol.  in  1  pt.  alcohol  at  15°. 
(Gautier  and  Charpy,  C.  R.  1890,  111. 
647.) 

100  g.  methyl  alcohol  dissolve  3.7  g.  HgI2 
at  19°;  ethyl  alcohol,  1.86  g.;  propyl  alcohol, 
1.25  g.;  isobutyl  alcohol,  at  22.5°,  0.51  g. 
(Timofeiew,  Dissert.  1894.) 

At  15-20°,  100  g.  methyl  alcohol  dissolve 
3.24  g.  HgI2;  ethyl  alcohol,  1.42  g.;  propyl 
alcohol,  0.826  g.  (Rohland,  Z.  anorg.  1898, 
16.  412.) 

Solubility  of  HgI2  in  ethyl  alcohol+Aq  at  25°. 

A  =  g.  alcohol  in  100  g.  alcohol+Aq. 

HgI2=millimols.  HgI2  in  100  cc.  of  the 
solution. 


A 

HgI2 

Sp.  gr. 

100 
95.82 
92.44 
86.74 

78.75 
67.63 

3.86 
2.56 
1.92 
1.38 
0.935 
0.45 

0.80325 
0.80950 
0.81536 
0.82996 
0.84654 
0.87214 

f  p 

HgI2 

Sp.  gr. 

70.01 
100 

0.061 
0.386 

0.8636 
0.8032 

(Herz  and  Knoch,  Z.  anorg.  1905,  45.  266.) 


Solubility  of  HgI2  in  methyl  alcohol+Aq  at 
25  . 

P  =  g.  alcohol  in  100  g.  alcohol+Aq. 
HgI2  =  millimols.   HgI2   in   10   cc.   of   the 
solution. 


p 

HgI2 

Sp.  gr. 

0 
47.06 
64.00 
78.05 
100 

0.0013 
0.0098 
0.0347 
0.0981 
0.571 

o!9is7 

0.8834 
0.8519 
0.8155 

(Herz  and  Anders,  Z.  anorg.  1907,  62.  165.) 


Solubility  of  HgI2  in  ethyl  alcohol+Aq  at  25°. 

P  =  g.  alcohol  in  100  g.  alcohol+Aq. 
HgI2  =  miUimols.  HgI2  in  10  cc.  of  the  solu- 
tion. 


(Herz  and  Anders,  Z.  anorg.  1907,  52.  170.) 


At  15°,  1  pt.  by  weight  is  sol.  in: — 
24813  pts.  H2O. 

30.8  pts.  methyl  alcohol  of  sp.  gr.  at  0.7990. 

70.3   "    ethyl  "       "   "     "'   "0.8100. 

121.0   "   propyl        "       "    "     "     "0.8160. 

(Rohland,  Z.  anorg.  1899,  18.  328.) 


Solubility  of  HgI2  in  mixtures  of  methyl  and 
ethyl  alcohol  at  25°. 

P  =  %  methyl  alcohol  in  the  mixtures. 
HgI2  =  g.  HgI2  in  10  com.  of  the  solution. 
S  25°/4°  =  Sp.  gr.  of  the  sat.  solution. 


P 

HgI2 

S  25°/4° 

0 

0.180 

0.8038 

4.37 

0.193 

0.8039 

10.4 

0.208 

0.8046 

41.02 

0.232 

0.8077 

80.69 

0.289 

0.8131 

84.77 

.       0.296 

0.8140 

91.25 

0.298 

0.8146 

100 

0.316 

0.8156 

(Herz  and  Kuhn,  Z.  anorg.  1908,  58.  164.) 

512 


MERCURIC  IODIDE 


Solubility  in  mixtures  of  methyl  and  propyl 
alcohol  at  25° 

Solubility  in  organic  solvents  at  t°. 

P  =  %  propyl  alcohol  in  the  solvent. 
G  =  g.  HgI2  in  10  ccm.  of  the  solution. 

Solvent 

t° 

100  g.  of  the 
solvent  dissolve 
g.  HgI2 

Q   Qri        rrr+       .rvf     fKj-v    n,n  f        «j-k1n  4  i.n.-n. 

r^Vi  1  nvnf  /~wm 

A1 

p 

G 

S  25°/4° 

v^moroiorm 
Tetrachlormethane 

Ol    • 

75 

.  163 
0.094 

0 

0.316 

0.8156 

Ethylene  dichloride 
Isobutyl  chloride 

85.5 
69 

1.200 
0.328 

23.8 

0.304 

0.8155 

Ethyl  bromide 

38 

0.773 

91.8 

0.169 

0.8101 

Methyl  alcohol 

66 

6.512 

93.75 
96.6 
100 

0.167 
0.153 
0.142 

0.8110 
0.8108 
0.8116 

Ethyl  alcohol 
Isopropyl  alcohol 
Isobutyl  alcohol 

78 
81 
ca.  100 

4.325 
2.266 
2.433 

(Herz  and  Kuhn,  Z.  anorg.  1908,  60.  158.) 

Methyl  formate 
Ethyl  formate 

36-38 
52-55 

1.166 
2.150 

Solubility  in  mixtures  of  propyl  and  ethyl 
alcohol  at  25° 

Methyl  acetate 
Ether 

56-59 
35 

2.500 
0.470 

P=  %  propyl  alcohol  in  the  solvent. 
G=g.  HgI2  in  10  ccm.  of  the  solution. 
S  =  Sp.  gr.  of  the  sat.  solution. 

Acetone 
Acetal 
Chloral 
Epichlorhydrin 

56 
ca.  100 
96 
ca.  100 

3.249 
2.000 

p 

G 

S  25°/4° 

Hexane 

67 

0.072 

Benzene 

80 

0  825 

0 

0.180 

0.8038  „ 

Ethyl  acetate 

74-78 

4.200 

.  1 
17.85 

.  173 
0.165 

0.8036(?) 
0.8043 

(Sulc,  Z.  anorg.  1900,  26.  402.) 

56  6 

0  155 

0  8075 

91.2 
95  2 

0.152 
0  144 

0.8099 
0  8108 

Solubility  in  organic  solvents  at   18-20°. 
100  g.  chloroform  dissolve  0.040  g.  HgI2. 

100 

0.142 

0.8116 

100  g.  tetrachlormethane  dissolve  0.006  g. 

(Herz  and  Kuhn,  Z.  anorg.  1908,  60.  161.) 

Solubility  in  100  pts.  amyl  alcohol  equals: 
0.66  pts.  at     13°. 
3.66    "     "     71°. 
5.30    "     "  100°. 
9.57    "     "  133.5°. 
(Laszcynski,  B.  1894,  27.  2287.) 

Sp.  gr.  at  16°/4°  of  HgI2+alcohol  contain- 
ing 1.8358%  Hglo  =  0.80718;  containing 
1.7119%  =0.80597.  (Schonrock,  Z.  phys. 
Ch.  1893,  11.  770.) 

.  Somewhat  sol.  in  ether.  Sol.  in  77  pts. 
ether.  (Saladin.)  Sol.  in  60  pts.  ether. 
(Hager.) 

Sol.  in  cold  ether.  (Francois,  J.  Pharm. 
1897,  (6)  6.  445.) 

Very  si.  sol.  in  anhydrous  ether.    (Hampe.) 

0.62  pt.  is  sol.  in  100  pts.  ether  at  0°. 

0.97  pt.  is  sol.  in  100  pts.  ether  at  36°. 
(Laszcynski,  B.  1894,  27.  2286.) 

Solubility  in  ether  =  0.3%  at  ord.  temp. 
(Marsh,  Chem.  Soc.  1910,  97.  2299.) 

Nearly  insol.  in  ether.  (Dunningham, 
Chem.  Soc.  1914,  105.  368.) 

Data  are  given  on  the  system  HgI2+KI  + 
ether.  (Dunningham.) 

Solubility  at  23°  in  chloroform  =  0.071%; 
in  ether  =  0.551%;  in  acetone  =  2. 005%:  in 
ethyl  alcohol  =2%;  in  methyl  alcohol  =. 
3.975%;  in  benzene  =  0.247%.  (Beckmann 
and  Stock,  Z.  phys.  Ch.  1895, 17. 130.) 


100  g.  bromoform  dissolve  0.486  g.  HgI2. 

100  g.  ethyl  bromide  dissolve  0.643  g. 
HgI2. 

100  g.  ethyl  iodide  dissolve  2.041  g.  HgI2. 

100  g.  ethylene  dibromide  dissolve  0.748  g. 
HgI2. 

(Sulc,  Z.  anorg.  1900,  25.  401.) 

1  pt.  ethylene  bromide  dissolves  0.00553 
pts.  HgI2  at  15°.  (Gautier  and  Charpy,  C.  R. 
1890,  111.  647.) 

100  pts.  methylene  iodide  CH2I2  dissolve 
2.5  pts.  HgI2  at  15°,  16.6  pts.  at  100°,  and  58 
pts.  at  180°.  (Retgers,  Z.  anorg.  3.  252.) 

1  1.  sat.  solution  in  CC14  at  15°  contains 
0.170  g.  HgI2.  (Dawson,  Chem.  Soc.  1909, 
95.  874.) 

Sol.  in  340  pts.  glycerine.  (Fairley,  Monit. 
Scient.  (3)  9.  685.)  • 

100  pts.  acetone  dissolve  2.09  pts.  HgI2  at 
25°.  (Krug  and  M'Elroy,  J.  Anal.  Ch.  6. 
84.) 

Sol.  in  acetone  and  in  methylal.    (Eidmann, 
C.  C.  1899,  II,  1014.) 
Solubility  in  100  pts.  acetone  equals: 
2. 83  pts.  HgI2  at    —  1°. 
3.36    "        "     "         18°. 
4.73    "        "     "        40°. 
6.07    "        "     "        58°. 
(Laszczynski,  B.  1894,  27.  2287.) 

100  g.  methyl  acetate  solution,  sat.  at  18°, 
contain  1.10  g.  HgI2.  (Bezold,  Dissert. 
1906.) 


MERCURIC  IODIDE 


513 


100  g.  boiling  methyl  acetate  slowly  dis- 
solve 2.3  g.  Hgl2.  (Schroeder  and  Steiner, 
J.  pr.  1909,  (2)  79.  49.) 


Solubility  in  ethyl  acetate  at  te 


Pts.  sol.  in  100  pts. 
ethyl  acetate 

t° 

1.49 

—  2 

1.56 

+  17.5 

1.64 

21 

2.53 

40 

3.19 

55 

4.31 

76 

(Laszczynski,  B.  1894,  27.  2286.) 


100  g.  ethyl  acetate  anhydrous,  or  sat. 
with  H2O  at  18°,  dissolve  at  18°,  14.70  g. 
Hgl2.  Solubility  increases  somewhat  with 
temp.  (Hamers,  Dissert.  1906.) 


Solubility  of  HgI2  in  ethyl  acetate +Aq  at  25°. 

P  =  g.  ethyl  acetate  in  100  g.  ethyl  acetate 
+Aq. 

HgI2  =  millimols.  HgI2  in  10  cc.  of  the 
solution. 


p 

HgI2 

Sp.  gr. 

4.39 
96.76 
100 

0.0028 
0.412 
0.241 

0.9973 
0.9063 
0.9011 

(Herz  and  Anders,  Z.  anorg.  1907,  52.  172. 


1  pt.  is  sol.  in  68.03  pts.  ethyl  acetate  at  18°. 
(Naumann,  B.  1910,  43.  316.) 

Solubility  in  diethyl  oxalate  is  12.5%  at 
bpt.  and  2.5%  at  100°.  (Reinders,  Z.  phys. 
Ch.  1900,  32.  507.) 


Solubility  in  CS2  at  t°. 


Solubility  in  CS2. 

100  g.  of  the  sat.  solution  contain  at: 

—86.5°        —93°        —116° 
0.024          0.023         0.017  g.  HgI2. 

(Arctowski,  Z.  anorg.  1896,  11.  274.) 

0.0028  pt.  is  sol.  in  1  pt.  CS2  at  15°.  (Gau- 
tier  and  Charpy,  C.  R.  1890,  111.  647.) 

1  1.  sat.  solution  in  CS2  at  15°  contains 
3.127  g.  HgI2.  (Dawson,  Chem.  Soc.  1909, 
95.  874.) 

Very  sol.  in  liquid  methylamine.  (Gibbs, 
J.  Am.  Chem.  Soc.  1906,  28.  1419.) 

Abundantly  sol.  in  methylamine.  (Fitz- 
gerald, J.  phys.  Chem.  1912,  16.  633.) 

Somewhat  sol.  in  allyl  mustard  oil.  (Math- 
ews,  J.  phys.  Chem.  1905,  9.  647.) 

Sol.inSb(CH3)4I+Aq. 

Very  si.  sol.  in  Na  citrate +Aq.    (Spiller.) 

1  pt.  C6H6  dissolves  0.00217  pts.  HgI2  at 
15°.  (Gautier  and  Charpy,  C.  R.  1890,  111. 
647.) 

Solubility  in  100  pts.  benzene  equals: 
0.22  pts.  at  15°. 
0.88     "    "  60°. 
0.95     "    "  65°.  • 
1.24     "    "84°. 
(Laszczynski,  B.  1894,  27.  2284.) 

1  1.  C6H6  dissolves  0.00493  mol.  HgI2  at 
25°.  (Sherrill,  Z.  phys.  Ch.  1903,  43.  735.) 

100  g.  boiling  phenol  dissolve  10  g.  HgI2. 
(Francois,  C.  R.  1895,  121.  769.) 

SI.  sol.  in  phenol  with  20%  H2O.  Not  very 
sol.  in  acetic  acid  at  119°,  in  amyl  acetate  at 
133°,  in  amyl  bromide  at  119°.  Rather  sol. 
in  diethyl  oxalate  at  186°,  in  ethylene  brom- 
ide at  131°,  in  amyl  alcohol  at  137°,  in  amyl 
iodide  at  150°,  in  CHBr3  at  151°,  in  iodo- 
benzol  at  190°,  in  oil  of  turpentine  at  160°. 
Very  sol.  in  benzaldehyde  at  179°,  in  methyl- 
ene  iodide  at  182°.  (Reinders,  Z.  phys.  Ch. 
1900,  32.  506.) 

1000  pts.  oil  of  bitter  almonds  dissolve  4 
pts.  HgI2  at  ord.  temp.;  1000  pts.  olive  oil, 
4  pts.;  1000  pts.  poppy  oil,  10  pts.;  1000  pts. 
nut  oil,  15  pts.;  1000  pts.  castor  oil,  20  pts.; 
1000  pts.  lard  oil,  4.  5  pts.;  1000  pts.  vaseline, 
2.5  pts.;  1000  pts.  benzene,  4  pts.  Sol.  in 
phenol.  (Mehn,  Pharm.  J.  3.  327;  B.  19.  8 


t° 

100  pts.  sat.  solution 
contain  pts.  Hgl2 

R.) 

Solubility  in  aniline. 
S  =  Temp.  of  solidification. 

—10 

0.107 
0.141 
0.173 
0.207 
0.239 
0.271 
0.320 
0.382 
0.445 

0 
+  5 
10 
15 
20 
25 
30 

Mols. 
per  100 

s 

Mols. 
per  100 

s 

Mols. 
per  100 

s 

5.9 
8.2 
10.3 
14.9 
16.6 

12° 
22.5 
29 
41.5 
45 

19.9 
25.8 
29.3 
31.7 
32.4 

48.5° 
53.5 
105 

122 

(55) 

33.0 
35.6 
37.5 
39.2 

128° 
140 
147 
156 

(Arctowski,  Z.  anorg.  1894,  6.  267.) 

(Staronka,  Anz.  Ak.  Wiss.  Krakau,  1910.  372.) 

514 


MERCURIC  IODIDE 


Solubility  of  HgI2  in  aniline  at  t°. 


t° 

g.  HgI2 
per  100  g. 
aniline 

Solid  phase 

—6.5 

23.35 

Hgl,  2C6H5NH2 

+0.4 

28.69 

it 

17.8 

42.85 

(( 

21.1 

47.55 

K 

26.9 

55.47 

(t 

30.1 

62.05 

ft 

36.2 

75.80 

11 

42.9 

96.49 

1C 

46.8* 

"  +HgI2(red) 

48.8 

128  '.I 

HgI2(red) 

63.6 

163.8 

(i 

70.  §2 

184.1 

(i 

76.2 

201.6 

(i 

95.9 

246.7 

it 

108.* 

HgI2(red)+HgI2(yellow) 

115.7 

28i!s 

HgI2(yellow) 

137.2 

285.2 

n 

181.1 

279 

n 

199.1 

863.2 

te 

*  Transition  point. 
(Pearce  and  Fry,  J.  phys.  Ch.  1914,  18.  667.) 


Very  sol.  in  boiling  alcoholic  solution  of 
aniline.  (Vohl,  Dissert.  1871.) 

Abundantly  sol.  in  hot  benzonitrile  and 
other  aromatic  nitriles.  (Werner,  Z.  anorg. 
1897,  16.  7.) 

Sol.  in  benzonitrile  (0.98  g.  in  100  g.  at 
18°).  20  times  more  sol.  by  addition  of 
5  g.  KI  to  100  cc.  benzonitrile.  (Naumann, 
B.  1914,  47.  1375.) 

Sol.  in  pyridine.  (Naumann,  B.  1904,  37. 
4609.) 


Solubility  of  HgI2  in  pyridine. 
S  =  temp.  of  solidification. 


Mols. 
per  100 

S 

Mols. 
per  100 

s 

Mols. 
per  100 

s 

5 

10° 

34.6 

107° 

51.3 

93.5° 

9.8 

42.5 

38.0 

103 

51.6 

96 

15.14 

66.5 

43.0 

97 

52.7 

108 

19.3 

83 

46.7 

88.5 

53.2 

109 

26.3 

102.5 

48.5 

89 

55.4 

122 

29.6 

107 

50.6 

89 

57.9 

135 

(Staronka,   Anz.   Ak.   Wiss.    Krakau,    1910. 

372.) 


Sp.  gr.  at  16°/4°  of  HgI2+pyridine  con- 
taining 10.43%  HgI2  =  1.1482;  containing 
7.99%  =  1.1053.  (Schonrock,  Z.  phys.  Ch. 
1893,  11.  770.) 


Solubility  of  HgI2  in  quinoline. 
temp,  of  solidification. 


Mols. 
per  100 

s 

Mols. 
per  100 

s 

Mols. 
per  100 

s 

4.7 

9.1 
13.2 
23.1 
26.7 

100° 
115.5 
133.5 
138 
145 

29.8 

31.4 
35.4 
37.7 
41.6 

151° 
153 
156 
160 
165 

43.0 
46.1 
48.8 
49.5 
54.4 

165° 
167 
170 
169.5 
166.5 

(Staronka,  Anz.  Ak.  Wiss.  Krakau,  1910.  372.) 


in     pyridine, 
(Werner,    Z. 


Mol.  weight  determined 
methyl-  and  ethyl-sulphide, 
anorg.  1897,  15.  20.) 

More  or  less  sol.  at  high  temp,  in  petroleum 
(bpt.  160-230°),  bromnaphthalene,  pyridine, 
toluidine  and  amyl  alcohol.     (Reinders,  Z. 
phys.  Ch.  1900,  32.  503.) 
Yellow   modification. 

100  g.  of  sat.  solution  in  acetone  at  25°  con- 
tain 3.0  g.  HgI2.     (Reinders,  Z.  phys.  Ch. 
1900,  32.  514.) 
Red  modification. 
Solubility  in  alcohol  equals: 
0.717-0.724  g.  in  100  g.  solution  at    0° 
1.044-1.084  g.         "  "         "  25° 

2.10-2.20  g.  "  50°. 

(Reinders,  Z.  phys.  Ch.  1900,  32.  522.) 

100  g.  of  sat.  solution  in  acetone  at  25° 
contain  1.95  g.  HgI2.  (Reinders,  Z.  phys. 
Ch.  1900,  32.  514.) 

HgI2  is  moderately  sol.  in  abs.  alcohol  at 
its  b.-pt.  The  solution  has  a  decided  yellow 
color.  On  cooling,  yellow  crystals  separate 
out.  They  soon  change  to  the  red  modifica- 
tion. 

Readily  sol.  in  hot  amyl  alcohol.  Yellow 
crystals  separate  from  the  solution  when 
cooled. 

Readily  sol.  in  allyl  alcohol,  forming  a 
yellow  solution,  from  which  yellow  crystals 
separate  on  cooling. 

SI.  sol.  in  acetone,  giving  a  yellow  solution. 
On  cooling  yellow  plates  separate  from  the 
solution  and  rapidly  turn  red. 

Sol  in  phenol  at  150°  C.  Solution  has  yel- 
low color  and  yellow  crystals  separate  out 
on  cooling. 

Readily  sol.  in  boiling  benzene.  Saturated 
solution  is  yellow.  The  yellow  iodide  sep- 
arates out  on  cooling,  and  changes  rapidly 
to  the  red. 

Sol.  in  toluene  giving  yellow  solution,  from 
which  yellow  crystals  separate  on  cooling. 
They  rapidly  change  to  red. 

Readily  sol.  in  naphthalene  at  temperatures 
above  its  transition  point.  Solution  is  yellow 
and  on  cooling  yellow  crystals  separate  out. 

Readily  sol.  in  hot  pseudo-cumene  giving 
a  yellow  solution.  On  cooling  gives  yellow 
crystals. 

Readily  sol.  in  ethyl  iodide  giving  very 


MERCURIC  SODIUM  IODIDE 


515 


yellow  solution,  from  which  yellow  crystals 
separate  on  cooling,  which  change  to  red 
rapidly. 

Only  si.  sol.  in  ethyl  bromide,  giving  yellow 
solution  from  which  yellow  crystals  separate 
on  cooling,  which  change  rather  slowly  to 
the  red. 

Sparingly  sol.  in  isopropyl  bromide. 

Moderately  sol.  in  isobutyl  bromide,  giving 
a  pink  solution  from  which  yellow  crystals 
separate  on  cooling,  which  change  slowly  to 
red. 

SI.  sol.  in  ethylidene  chloride.  On  sudden 
cooling  at  18°  the  iodide  crystallizes  out  in 
yellow  plates,  which  quickly  change  to  red. 

Sparingly  sol.  in  propyl  chloride,  giving  a 
pink  solution,  from  which  yellow  crystals 
separate  on  cooling. 

Readily  sol.  in  ethyl  cyanide,  giving  a 
yellow  solution.  On  cooling  yellow  crystals 
separate  and  rapidly  change  to  red. 

Moderately  sol.  in  benzene  cyanide,  giving 
a  deep  yellow  solution.  On  sudden  cooling 
the  solution  deposits  yellow  crystals,  which 
rapidly  turn  red. 

Rapidly  sol.  in  benzoic  acid  at  high  tem- 
peratures. 

Sparingly  sol.  in  ethyl  acetate,  giving 
yellow  solution. 

Sol.  in  ethyl  propionate. 

Very  sol.  in  ethyl  butyrate,  giving  a  yellow 
solution.  On  cooling  the  iodide  crystallized 
from  the  solution. 

SI.  sol.  in  ethyl  isobutyrate. 

Readily  sol.  in  methyl  salicylate,  giving 
a  yellow  solution. 

Sparingly  sol.  in  phenyl  salicylate,  giving 
yellow  solution.  On  cooling  yellow  crystals 
separate  out,  which  gradually  change  to  red. 
(Kastle,  Am.  Ch.  J.  1899,  22.  474.) 

Mercuromercuric  iodide.  Hg4l6  =  Hg2l2, 

2HgI2. 

Insol.  in  H2O  or  alcohol.  Partially  sol.  in 
KI+Aq,  in  hot  NaCl,  and  NH4Cl+Aq,  and 
in  hot  HCl+Aq,  though  Very  slowly.  (Boul- 
lay,  A.  ch.  (2)  34.  345. 


Mercury  periodide, 

Sol.  in  KI+Aq.  Decomp.  by  cold  H2O  or 
alcohol.  (Jorgensen,  J.  pr.  (2)  2.  347.) 

Mercuric    hydrogen    iodide     (lodomercuric 

acid),  HI,  HgI2=HHgI3. 
Crystallises  from  Hl-f  Aq.     (Boullay.) 
Easily  decomp.    (Neumann,  M.  10.  236.) 
3HgI2,    2HI+H2O.      (Francois,    Dissert. 

1901.) 

Mercuric  nickel  iodide,  HgI2,  NiI2+6H2O. 

Sol.  in  alcohol,  ether,  and  acetone;  not 
decomp.  by  H2O.  (Dobroserdoff,  C.  C.  1901, 
11.332.)  " 

2HgI2,  NiI2+6H2O.  Hydroscopic;  decomp. 
by  H2O  ;  sol.  in  acetone  and  ether.  (Dobroser- 
doff, C.  C.  1901,  II.  332.) 


Mercuric    potassium    iodide,    HgI2,     KI  + 


Deliquescent  (v.  Bonsdorff).  Permanent; 
decomp.  by  H2O  into  2KI,  HgI2,  and  HgI2 
(Boullay);  sol.  in  alcohol,  ether,  and  cone. 
HC2H3O2,  but  decomp.  by  other  acids  (Ber- 
thempt,  J.  Pharm.  14.  186).  Sp.  gr.  of  sat. 
solution  in  H2O  =2.4  to  3.1. 

+H2O.  Sol.  in  H2O  with  decomp.  Can 
be  cryst.  from  alcohol.  Very  si.  sol.  in  dry 
ether.  Very  sol.  in  wet  ether.  (Marsh,  Chem. 
Soc.  1910,  97.  2297.) 

HgI2,  2KI.  Sol.  in  H2O.  (Thomsen  and 
Bloxam,  Chem.  Soc.  41.  379.) 

Sat.  solution  of  KI-f-HgI2  in  H2O  at  22.9° 
contains  8.66%  K,  22.49%  Hg  and  52.48%  I, 
corresponding  to  0.22  mol.  K,  0.11  mol.  Hg 
and  0.45  mol.  I.  (Duboin,  C.  R.  1905,  141. 
385.) 

Sp.  gr.  at  16°  /4°  of  aqueous  solution  con- 
taining 12.2875%  salt  =  1.10148;  containing 
12.2371%  =  1.1038;  containing  7.9843%  = 
1.06491.  (Schonrock,  Z.  phys.  Ch.  1893,  11. 
782.) 

Sol.  in  methyl  acetate.  (Bezold,  Dissert. 
1906.) 

Sol,  in  ethyl  acetate.  (Alexander,  Dissert. 
1899;  Hamers,  Dissert.  1906.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4328.) 

Sol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1904,  37.  3601.) 

+2H2O.  Sol.  in  alcohol,  ether  and  acetone; 
decomp.  by  H2O.  (Pawlow,  C.  C.  1901,  I. 
363.) 

Solubility  determinations  show  that  KHgI3 
and  KHgI3+H2O  are  the  only  double  salts 
formed  at  20°-30°.  See  HgI2+KI  under 
HgI2.  (Dunningham,  Chem.  Soc.  1914,  105. 


Mercuric  rubidium  iodide,  HgI2,  Rbl. 

Sol.  in  alcohol;  decomp.  by  H2O. 

HgI2,  2RbI.  Very  easily  sol.  in  H2O. 
(Grossmann,  B.  1904,  37.  1258.) 

Very  sol.  in  acetic  acid  and  alcohol;  decomp. 
by  H2O.  Stable  in  aq.  solution  in  the  pres- 
ence of  an  excess  of  Rbl.  (Erdmann,  Arch. 
Pharm.  1894,  232.  30.) 

Mercuric  silver  iodide,  HgI2,  2AgI. 

(Wegelius  and  Kilpi,  Z.  anorg.  1909,  61. 
416.) 

Mercuric  sodium  iodide,  HgI2,  Nal. 

Deliquescent,  and  decomp.  by  much  H2O. 
(v.  Bonsdorff  Pogg.  17.  266.) 

Sol.  in  alconol;  decomp.  by  H2O. 

HgI2,  2NaI.  Deliquescent;  sol.  in  H2O  and 
alcohol.  (Boullay.) 

Sat.  solution  of  NaI+HgI2  in  H2O  at 
24.75°  contains  4.59%  Na,  25%  Hg,  and 
58.25%  I,  corresponding  to  0.20  mol.  Na, 


516 


MERCURIC  STRONTIUM  IODIDE 


0.12  mol.  Hg,  and  0.45  mol.  I.    (Duboin,  C.  R. 

1905,  141.  385.) 

+4H2O.  Extremely  deliquescent.  (Du- 
boin, C.  R.  1906,  143.  314.) 

Mercuric  strontium  iodide,  HgI2,  SrI2  (?). 
Sol.  in  H2O  without  decomp.    (Boullay.) 
+8H2O.     As   Ca  salt.     (Duboin,   C.   R. 

1906,  142.  573.) 

2HgI2,  Srl2  (?).  Decomp.  by  much  H2O 
into  sol.  HgI2,  SrI2  and  insol.  HgI2.  (Boul- 
lay.) 

Mercuric    thorium    iodide,     5HgI2,    ThI4  + 

18H2O. 
Very    deliquescent.      Easily    decomp.    by 

H2O.    (Duboin,  A.  ch.  1909,  (8)  16.  282.) 
5HgI2,  2ThI4+21H2O.    (Duboin.) 
2HgI2,  ThI4  +  12H2O.    (Duboin.) 

Mercuric  zinc  iodide. 

Deliquescent.  Decomp.  by  H2O.  (v. 
Bonsdorff.) 

Mercuric  iodide  ammonia,  HgI2,  2NH3. 

Decomp.  by  NH3  giving  NHg2I  and  NH4I. 
(Francois,  C.  R.  1900,  130.  333.) 

Stable  only  in  the  presence  of  excess  of 
ammonia.  Gives  off  NH3  in  the  air.  (Fran- 
cois, J.  Pharm.  1897,  (6)  5.  388;  C.  C.  1897, 
I.  1088.) 

Mercuric  iodide  hydrazine,  HgI2,  N2H4. 

Decomp.  by  H2O.  (Hofmann  and  Mar- 
burg, A.  1899,  306.  215.) 

Mercuric  iodide  rubidium  bromide, 
HgI2,  2RbBr. 

Decomp.  by  H2O. 

Sol.  in  alcohol  without  decomp.  (Gros- 
mann,  B.  1903,  36.  1603.) 

Mercuric  iodide  silver  chloride,  HgI2,  2AgCl. 
Insol.  in  H2O.     (Lea,  Sill.  Am.  J.  (3)  7. 
34.) 

Mercury  iodoantimonide,   Hg3Sb42HgI2. 

Sol.  in  HNO3  aqua  regia  and  hot  H2SO4; 
insol.  in  HC1.  (Granger,  C.  R.  1901,  132. 
1116.) 

Mercury  nitride,  Hg3N2. 

Gradually  decomp.  by  H2O.  Decomp.  by 
cone.  HNO3,  or  HCl+Aq.  (Hirzel,  J.  B. 
1852.419.) 

Not  attacked  by  cold,  but  decomp.  by  hot 
dil.  H2S04. 

Sol.  in  acids +Aq. 

Sol.  in  ammoniacal  solutions  of  ammonium 
salts. 

Insol.  in  excess  of  KNH3.  (Franklin,  Z. 
anorg.  1905,  46.  18.) 

Sol.  in  ammonia  solutions  of  ammonium 
salts  and  in  aq.  acid  solutions. 


Very  explosive.     (Franklin,  J.  Am.  Chem. 
Soc.  1905,  27i  835.) 
HgN3. 

See  Mercurous  azoimide. 
HgN6. 
See  Mercuric  azoimide. 


Mercurous  oxide,  Hg2O. 

Insol.  in  H2O.  Insol.  in  dil.  HC1  or  HNO3 
+Aq.  Sol.  in  warm  cone.  HC2H3O2+Aq. 

Sol.  in  150,000  pts.  H2O.  (Bhaduri.  Z. 
anorg.  1897,  13.  410.) 

Decomp.  by  H2O  or  weak  bases  (Rose), 
(NH4)2CO3+Aq  (Wittstein),  KNO3+Aq 
(Rose),  KI+Aq  (Berthemot),  or  cone. 
NH4Cl-fAq  (Pagenstecher)  into  HgO  and 
Hg,  or  HgCl2,  etc. 

SI.  decomp.  by  alkali  chlorides +Aq  with 
formation  of  HgCl2,  which  dissolves. 
(Miahle.) 

SI.  sol.  in  alkali  cyanides +Aq.     (Jahn.) 

Insol.  in  KOH,  and  NaOH+Aq. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Insol.  in  alcohol  and  ether. 

Mercuric  oxide,  HgO. 

Sol.  in  20,000  to  30,000  pts.  H2O.  (Bineau, 
C.R.41.509.) 

Sol.  in  200,000  pts.  H2O.  (Wallace,  Ch. 
Gaz.  1858.  345.) 

Ordinary  coarse  HgO  is  sol.  in  H2O  to 
the  extent  of  50  mg.  per  1.  at  25°,  but  when 
finely  powdered  the  solubility  increases  to 
150  mg.  per  1.  (Hulett,  Z.  phys.  Ch.  1901, 
37.  406.) 

Red  modification  is: — 

Sol.  in  19,500  pts.  H2O  at  25°;  in  2,600  pts. 
H2O  at  100°.  (Schick,  Z.  phys.  Ch.  1903, 
42.  172.) 

1  1.  H20  dissolves  50  mg.  red  modification 
of  HgO  at  25°.  (Hulett,  Z.  phys.  Ch.  1901, 
37.406.) 

Yellow  modification  is: — 

Sol.  in  19,300  pts.  H2O  at  25°;  in  2400  pts. 
at  100°.  (Schick,  Z.  phys.  Ch.  1903,  42. 
172.) 

Sol.  in  acids.  Insol  in  H3PO4  or  H3AsO4  + 
Aq.  (Haack,  A.  262.  190.) 

Scarcely  attacked  by  H2C2O4+Aq.  (Mil- 
Ion,  A.  ch.  (3)  18.  352.) 

Solubility  of  HgO  in  HF  at  25°. 
Hg  =  g.-atoms  Hg  in  1  1.  of  the  solution. 


HF  normal 

Hg 

0.12 
0.24 
0.57 
1.11 
2.17 

0.01258 
0.0247 
0.0629 
0.1168 
0.2586 

(Jaeger,  Z.  anorg.  1901,  27.  26.) 


MERCURIC  OXYCHLORIDE 


517 


Solubility  of  HgO  in  HF  is  decreased  by  the 
addition  of  KF,  which  proves  the  non- 
existence  of  complex  fluorides.  (Jaeger.) 

Insol.  in  H3AsO4,  H3PO4  and  in  primary 
and  secondary  alkali  salts  of  these  acids. 
(Haack,  A.  1891,  262.  190.) 

Sol.  in  hot  NH4Cl+Aq,  less  in  NH4NO3  + 
Aq.  (Brett.) 

Insol.  in  KOH,  or  NaOH+Aq. 

Decomp.  by  alkali  chlorides +Aq  into 
HgCl2,  which  dissolves*  (Miahle,  A.  ch. 
(3)  5.  177.) 

Sol.  in  Fe(NO3)3,  and  BifNO3)3+Aq  with 
pptn.  of  oxides.  Sol.  in  Kl-f  Aq.  (Persoz.) 

Very  sol.  in  acid  sulphites +Aq.  (Earth, 
Z.  phys.  Ch.  1892,  9.  192.) 

Completely  sol.  in  cone.  CaCl2,  BaClo, 
MgCl2,  and  SrCl2+Aq.  (Andre,  C.  R.  1887, 
104.  431.) 

Solubility  in  Ag  salts +Aq.  100  g.  Ag2SO4 
in  aqueous  solution  dissolve  13  g.  HgO.  Sol- 
ubility in  AgNO3+Aq  is  15.6  : 100;  in  Ag 
acetate+Aq  is  1.137:100.  (Finci,  Gazz. 
ch.  it.  1911,  41.  (2)  545.) 

Much  less  sol.  in  KC1  and  NaCl+Aq 
than  in  H2O.  (Schoch.) 

Sol.  in  U(NO3)3,  A1(NO3)3  and  Fe(NO3)3  + 
Aq.  (Mailhe,  A.  ch.  1902,  (7)  27.  373.) 

Very  si.  sol.  in  cold  Hg(CN)2-f-Aq,  abun- 
dantly sol.  at  75°  with  evolution  of  HCN. 
(Barthe,  J.  Pharm.  1896,  (6)  3.  183.) 

Sol.  in  cold  or  hot  alcoholic  NH4SCN  in 
large  amounts.  (Fleischer,  A.  1875,  179. 
225.) 

Completely  sol.  in  KI+Aq.  (Jehn,  Arch. 
Pharm.  1873,  201.  97.) 

Solubility  of  red  or  yellow  modification  in 
N/50  KCl+Aq  is  about  25%  greater  than 
in  pure  H2O.  (Schick,  Z.  phys.  Ch.  1903,  42. 
168.) 

Insol.  in  liquid  HF. 
1905,  46.  2.) 

Insol.  in  liquid  NH3 
1898,  20.  829.) 

Insol.  in  liquid  NH3. 
J.  1898,  20. 829.) 

Sol.  in  alcoholic  solution  of  hydroxylamine 
hydrobromide  below  0°.  (Adams,  Am.  Ch. 
J.  1902,  28.  216.) 

Insol.  in  alcohol. 

Sol.  in  trichloracetic  acid+Aq.  (Brand, 
J.  pr.  1913,  (2)  88.  342.) 

Insol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

Insol.  in  acetone.     (Naumann,   B.    1904, 

37.  4329.) 

When  freshly  pptd.,  is  insol.  in  acetone + 
Aq.  even  on  warming,  but  easily  sol.  if  liquid 
is  made  alkaline  by  NaOH.  Insol.  in  aceto- 
phenone  even  after  long  warming  at  100°. 
Sol.  in  acetaldehyde  and  much  H2O  and  a 
little  NaOH.  (Auld  and  Hantzsch,  B.  1905, 

38.  2680.) 

Sol.  in  formamide.  (Fischer,  Arch.  Pharm. 
1894,  232.  329.) 

Very  sol.  in  ethylene  diamine.    For  1  mol. 


(Franklin,  Z.  anorg. 
(Gore,  Am.  Ch.  J. 
(Franklin,  Am.  Ch. 


HgO,  7-10  mols.  ethylene  diamine  are  neces- 
sary. (Traube  and  Lowe,  B.  1914,  47.  1910.) 

Easily  sol.  in  benzamide.  (Dessaignes, 
A.  ch.  1852,  (3)  34. 146..) 

When  freshly  pptd.,  is  sol.  in  picric  acid  + 
Aq.  (Varet,  C.  R.  1894,  119.  560.) 

Sol.  in  alkaline  solution  of  phenol  disul- 
phonic  acid.  (Lumiere  and  Chevrotier,  C.  R. 
1901,  132.  145.) 

Sol.  in  nucleic  acid+Aq  when  freshly 
pptd.  (Schweckerath,  Pat.  1899.) 

Sol.  in  gum  arabic+Aq.  (Peschier,  J. 
Pharm.  1896,  (6)  3.  509.) 

Mercuric  oxybromide,  HgBr2,  HgO. 

(Andre,  An  ch.  (6)  3.  123.) 

HgBr2,  2HgO.    (Andre.) 

HgBr2,  3HgO.  (a)  Yellow.  Insol.  in  cold, 
si.  sol.  in  hot  H2O.  Easily  sol.  in  alcohol. 
(Lowig.) 

(6)  Brown.  Insol.  in  alcohol.  (Rammels- 
berg,  Pogg.  55.  248.) 

HgBr2,  4HgO.    (Andre.) 

Insol.  in  ord.  solvents.  Decomp.  by  al- 
kalies and  acids.  (Fischer  and  von  Warten- 
burg,  Ch.  Z.  1902,  26.  894.) 

2HgBr2,  7HgO.  Readily  decomp.  by  acids 
and  alkalies.  (Fischer  and  von  Wartenburg.) 

Mercurous  oxychloride,  Hg2O,  2HgCl. 

Min.     Egleslonite. 

Decomp.  by  hot  HC1  and  by  HNO3. 
(Moses,  Am.  J.  Sci,  1903,  (4)  16.  253.) 

Mercuric  oxychloride, 

HgO,  HgCl2.  Less  sol.  than  HgCl2,  but 
not  isolated.  (Thummel.)  Decomp.  by 
cold  H2O.  (Andre,  A.  ch.  (6)  3.  118.) 

HgO,  2HgCl2.  Decomp.  by  warm  H2O  or 
cold  alcohol  into  2HgO,  HgCl2.  (Thummel, 
Arch.  Pharm.  (3)  27.  589.) 

Decomp.  by  H2O.  Not  decomp.  by  al- 
cohol. (Arctowski,  Z.  anorg.  1895,  9.  178.) 

2HgO,   HgCl2.    Two  modifications. 

A.  Red.    Insol.  in  H2O;  decomp.  by  alkali 
carbonates,    or    chlorides +Aq    into    4HgO. 
HgCl2. 

Acted  upon  by  cold  alkali  carbonates  and 
alkali  chlorides +Aq.  (Schoch,  Am.  Ch.  J. 
1903,  29.  335.) 

Not  decomp.  by  H2O  at  ord.  temp.  (Thum- 
mel.) 

Very  si.  sol.  in  cold,  completely  sol.  in 
hot  H2O.  (Haack,  A.  1891,  262.  189.) 

A  small  amt.  of  HNO3  converts  it  into  a 
white  powder;  more  HNO3  dissolves  it. 
(Haack,  A.  1891,  262.  189.) 

B.  Black.    Not  decomp.  by  alkali  chlorides, 
or  carbonates +Aq.    (Thummel.) 

Not  affected  by  boiling  alkali  carbonates 
or  alkali  chlorides  +Aq.  (Schoch,  Am.  Ch. 
J.  1901,  29.  335.) 

Insol.  in  cold  and  hot  H2O  and  alcohol. 

Sol.  in  acid.    (Van  Nest,  Dissert.  1909.) 

Not  changed  by  H2O.  (Blaas,  Miner 
Mitt.  (2)  2.  177.) 


518 


MERCUROMERCURIC  OXYCHLORIDE 


Sol.  in  HNO3  or  HCl+Aq.  fc  (Blaas.) 
Not  changed  bv  alcohol.    (Blaas.) 
+  i£E2O.    (Ray,  A.  1901,  316.  255.) 
3HgO,  HgCl2.     Decomp.  by  warm  H2O. 
(Thiimmel.) 

Not  attacked  by  cold  H2O.     (Andre.) 
Ppt.    (Tarugi,  Gazz.  ch.  it.  1901,  31.  313.) 
Decomp.  by  H2O.     Not  decomp.  by  al- 
cohol.   (Arctowski,  Z.  anorg.  1895,  9.  178.) 
Three  modifications. 

a.  Prisms.    Decomp.  by  boiling  H2O. 

b.  Brick-red,  amorphous. 

c.  Yellow  plates. 

(Schoch,  Am.  Ch.  J.  1903,  29.  337.) 

Yellow  plates. 

Decomp.  by  hot  H2O,  Na2CO3  or  NaOH  + 
Aq.  Sol.  in  KHCO3+Aq.  Insol.  in  cold  dil. 
HNO3.  (Tarugi.) 

4HgO,  HgCl2.  Decomp.  by  H2O.  Not 
decomp.  by  alcohol.  (Arctowski,  Z.  anorg. 
1895,  9.  178.) 

Two  modifications. 

A.  Yellow  plates. 

Easily  sol.  in  acids.  Insol.  in  alcohol  and 
ether.  Decomp.  by  KOH.  (Dukelski,  Z. 
anorg.  1906,  49.  336.) 

B.  Brown,  amorphous. 

Easily  sol.  in  acids.     Decomp.  by  KOH. 

Insol.  in  alcohol  and  ether.  (Dukelski, 
Z.  anorg.  1906,  49.  336.) 

5HgO,  HgCl2.    (Millon.) 

Does  not  exist.    (Thiimmel.) 

6HgO,  HgCl2.    Does  not  exist.    (T.) 

+H2O.  Insol.  in  cold  H2O.  (Roucher,  A. 
ch.  (3)  27.  353.) 

Does  not  exist.    (T.) 

7HgO,  4HgCl2.    (Roucher.) 

Does  not  exist.    (T.) 

Mercuromercuric  oxychloride,  Hg2OCl. 

Min.  Terlinguaite. 

Decomp.  by  HC1  and  HNO3. 

Slowly  decomp.  by  cold  acetic  acid  when 
powdered.  (Hillebrand  and  Schaller,  J. 
Am.  Chem.  Soc.  1907,  29.  1190.) 

Mercuric  strontium  oxychloride.  HgO,  SrCl2 

+6H2O. 
Decomp.  by  H2O.    (Andre,  C.  R.  104.  431.) 

Mercuric  oxyfluoride,  HgO,  HgF2+H2O. 

Decomp.  by  H2O.  Sol.  in  dil.  HNO3+Aq. 
(Finkener.) 

Mercuric  oxyiodide,  3HgO,  HgI2. 

Decomp.  by  H2O.  Sol.inHI+Aq.  (Weyl, 
Pogg.  131.  524.) 

Mercuric  oxyphosphide,  Hg5P2O4. 

Decomp.  by  H2O.  (Partheil  and  van 
Haaren,  Arch.  Pharm.  1900,  238.  35.) 

Mercuric  oxyselenide,  2HgSe,  HgO. 

Easily  sol.  in  aqua  regia.  (Uelsmann,  A. 
116.  122.) 


Mercury  phosphide,  Hg3P2. 

Insol.  in  H2O,  HNO3,  or  HCl+Aq.  Easily 
sol.  in  aqua  regia.  (Granger,  C.  R.  115.  229.) 

Hg3P4.    (Granger,  C.  N.  1898,  77.  229.) 

Mercury  phosphochloride,  P2Hg3,  3HgCl2  + 

3H2O. 

See    Drniercuriphosphonium    mercuric 
chloride. 

Mercury  phosphosujphide,   2HgS,    P2S. 
HgS,  P2S. 

2HgS,  P2S3.     (Berzelius.) 
3HgS,  P2S3.    (Baudrimont,  C.  R,  56.  323.) 
2HgS,  P2S5.     (Berzelius,  A.  47.  256.) 

Mercuric  selenide,  HgSe. 

Sol.  in  cold  aqua  regia  when  crystalline. 
When  precipitated  shows  the  same  properties 
towards  solvents  as  mercuric  sulphide.  (Reeb 
J.  Pharm.  (4)  9.  173.) 

Min.  Tilmannite.    Sol.  only  in  aqua  regia. 

Mercuric  selenochloride,  2HgSe,  HgCl2. 

Insol.  in  boiling  HC1,  HN03,  or  H2SO4+ 
Aq.  Easily  sol.  in  aqua  regia  and  a  mixture 
of  H2SO4  and  cone.  HNO3+Aq.  (Uelsmann, 
J.  B.  1860.  92.) 

Mercurous  sulphide,  Hg2S. 

Insol.  in  H2O,  dil.  HNO3,  hot  NH4OH,  or 
(NH4)2S+Aq.  Sol.  in  KOH  +Aq  with  separa- 
tion of  Hg.  (Rose.) 

Does  not  exist;  only  mixtures  of  Hg  and 
HgS  are  formed.  (Barfoed,  J.  pr.  93.  230.) 

See  also  Baskerville,  J.  Am.  Chem.  Soc. 
1903,  25.  799.) 

Not  attacked  by  HNO3  below  0°,  but  at- 
tacked by  dil.  HNO3  and  HCl+Aq  when 
temp,  is  increased.  Sol.  in  Na2S  or  K2S  but 
Hg  soon  ppts.  (Antony  and  Sestini,  Gazz. 
ch.  it.  1894,  24,  (1)  194.) 

Mercuric  sulphide,  HgS. 

Insol.  in  H2O. 

Pptd.  as  a  brown  coloration  in  presence  of 
20,000  pts.  H2O,  and  as  a  green  coloration  in 
presence  of  40,000  pts.  H2O.  (Lassaigne.) 

Much  less  sol.  in  H2O  than  Ag2S  or  Cu2S. 
(Bodlander,  Z.  phys.  Ch.  1898,  27.  64.) 

11..  H2O  dissolves  0.05  X10-6  mols  HgS  at 
18°.  (Weigel,  Z.  phys.  Ch.  1907,  58.  294.) 

Sol.  in  cold  cone.,  and  in  hot  dil.  HI+Aq  or 
HBr+Aq.  (Kekule,  A.  Suppl.  2.  101.)  Very 
si.  decomp.  by  hot  cone.  HCl+Aq.  Not  at- 
tacked by  hot  HNO3+Aq.  Sol.  in  cold  aqua 
regia. 

Not  attacked  by  4-N  HNO3  or  4^N  HNO3 
+4-N  H2SO4  at  ord.  temp,  even  after  many 
days.  By  action  of  a  mixture  of  equal  volumes 
of  4-N  HNO3  and  cone.  H2SO4,  there  was 
slight  action  on  pptd.  HgS  after  14,  more 
action  after  62  days.  If  HgS  is  boiled  with 
the  4-N  acids,  oxidation  takes  place  most 
rapidly  with  4-N  HNO3,  then  the  mixture 
66.7%  4-N  H2SO4+33.3%  4-N  HNO3,  then 


MERCURIC  SULPHOIODIDE 


519 


33.3%  4-N  H2SO4+66.7%  4-N  HNO3,  and 
lastly  4-N  H2SO4  alone.  (Moore,  J.  Am. 
Chem.  Soc.  1911,  33.  1094.) 

Cold  cone.  H2SO4  does  not  attack  red  or 
black  HgS,  but  they  are  attacked  by  hot  acid. 
(Berthelot,  A.  ch.  1898,  (7)  14.  198.) 

Freshly  pptd.  HgS  is  insol.  in  dil.  KCN  + 
Aq.  (Berthelot.) 

Sol.  in  K2S+Aq,  but  readily  only  in  pres- 
ence of  free  alkali.  (Brunner,  Pogg.  15.  596.) 
Insol.  in  boiling  KOH+Aq. 

Sol.  in  KSH  or  NaSH+Aq.  Very  si.  sol. 
in  cold  yellow  (NH4)2S+Aq.  Insol.  in  KCN 
or  Na2S2O3+Aq.  (Fresenius.) 

Easily  sol.  in  cone.  Na2S  or  K2S+Aq, 
even  in  absence  of  KOH  or  NaOH.  Insol.  in 
(NH4)2S+Aq.  Sol.  in  CaS,  BaS,  or  SrS+Aq. 
Insol.  in  NaSH  or  KSH+Aq.  (de  Koninck, 
Z.  angew.  Ch.  1891.  51.) 

Solubility  in  NaSH  is  very  small  in  com- 
parison with  that  in  Na2S+Aq.  (Knox, 
Trans.  Faraday.  Soc.  1908,  4.  30.) 

Solubility  in  BaS  is  practically  equal  to 
thatinNa2S.  (Knox.) 

All  cryst.  modifications  are  sol.  in  cone. 
K2S  and  in  cone.  Na2S+Aq.  (Allen  and 
Crenshaw,  Am.  J.  Sci.  1912,  (4)  34.  368.) 

Sol.    in    potassium    thiocarbonate+Aq. 
(Rosenbladt,  Z.  anal.  26.  15.) 

Sol.  in  alkali  sulpho-molybdates,  -tung- 
states,  -vanadates,  -arsenates,  -antimonates, 
and  -stannates.  (Storch,  B.  16.  2015.) 

1  1.  BaS2H2+Aq  containing  50  g.  Ba  dis- 
solves no  HgS  in  the  cold,  but  50-60  g.  at 
40-50°. 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  829.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014.) 

Insol.  in  pyridine.  (Schroeder,  Dissert. 
1901.) 

Insol:  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

Exists  in  a  colloidal  state,  sol.  in  H2O. 
(Winnsinger,  Bull.  Soc.  (2)  49.  452.) 

Min.  Cinnabar.  Insol.  in  H2O,  alcohol, 
dil.  acids,  or  alkaline  solutions. 

Decomp.  by  hot  dil.  HNO3+Aq.  Not 
decomp.  by  HCl+Aq,  but  easily  by  hot 
H2SO4  or  aqua  regia.  Easily  sol.  in  CuCl2  + 
Aq.  (Karsten.) 

Sol.  in  a  mixture  of  Na2S  and  NaOH  when 
present  in  the  proportion  of  HgS  :  2Na2S. 

Sol.  in  pure  Na2S-f-Aq  or  in  mixtures  of 
Na2S  and  NaSH+Aq.  Insol.  in  cold  NaSH  + 
Aq,  but  sol.  on  warming  with  evolution  of 
H2S.  (Becker,  Sill.  Am.  J.  (3)  33.  199.) 

Insol.  in  acetone.    (Krug  and  M'Elroy.) 

Cinnabar  is  easily  sol.  in  20%  HBr+Aq. 
(Rising  and  Lenher,  J.  Am.  Chem.  Soc.  1896, 
18.  96.) 

Sol.  in  S2C12.  (Smith,  J.  Am.  Chem.  Soc. 
1898,  20.  291.) 

Mercuric  platinum  sulphide. 
See  Sulphoplatinate,  mercuric. 


Mercuric  potassium  sulphide,  K2S,  2HgS. 

Decomp.  into  its  constituents  by  H2O;  de- 
comp. by  HC1,  and  HNO3+Aq,  and  by  hot 
KOH,  and  NH4OH+Aq.  (Schneider,  Pogg. 
127.  488.) 

K2S,  HgS+5H2O.  Decomp.  by  H2O  or 
alkalies.  (Weber,  Pogg.  97.  76.) 

+H2O.    (Ditte.) 

+7H2O.  Sol.  in  K2S+Aq.  (Ditte,  C.  R. 
98.  1271.) 

K2S,  5HgS+5H2O.  Easily  decomp.  by 
H2O.  (Ditte.) 

Mercuric  sodium  sulphide,  HgS,  Na2S+ 
8H2O. 

Decomp.  by  H2O  or  alkalies. 

5HgS,  2Na2S+3H2O.  Decomp.  by  H2O. 
(Knox,  Trans.  Faraday  Soc.  1908,  4.  36.) 

Mercuric  sulphobromide,  2HgS,  HgBr2. 

Insol.  in  H2O.  Not  attacked  by  boiling 
HNO3orH2SO4.  (Rose.) 

Mercuric  sulphochloride,  2HgS,  HgCl2. 

Insol.  in  H2O,  cold  or  hot,  dil.  or  cone. 
HNO3,  H2SO4,  or  HCl+Aq.  (Rose,  Pogg.  13. 
59.) 

Decomp.  by  hot  aqua  regia. 

By  boiling  with  dil.  HNO3,  H2SO4  and 
HC1,  Hg  and  Cl  go  into  solution.  (Hamers, 
Dissert.  1906.) 

Insol.  in  H2O  and  H2SO4.  Partly  sol.  in 
HC1  and  HNO3;  easily  sol.  in  aqua  regia. 
(Alexander,  Dissert.  1899.) 

Sol.  in  aqua  regia.  (Deniges,  Bull.  Soc. 
1915,  (4)  17.  356.) 

3HgS,  HgCl2.  Properties  as  the  above 
comp.  (Poleck  and  Goercki,  B.  21.  2415.) 

4HgS,  HgCl2.    As  above.    (P.  and  G.) 

5HgS,  HgCl2.    As  above.    (P.  and  G.) 

Insol.  in  alkali  sulphides  and  in  fuming 
HNO3;  decomp.  by  NaOBr+Aq  and  by 
KOH.  (Bodroux,  C.  R.  1900,  130.  1399.) 

SI.  sol.  in  solutions  of  alkali  sulphides  unless 
heated.  (Berzelius.) 

Easily  sol.  in  alkali  sulphides  +Aq;  slowly 
sol.  in  alkalies  or  alkali  hydrosulphides+Aq. 
(Atterberg,  J.  B.  1873.  258.) 

Mercurous  sulphotetra chloride,  Hg2SCl4. 

Decomp.  by  H2O  with  separation  of  S, 
HgCl2  going  into  solution.  (Capitaine,  J. 
Pharm.  25.  525.) 

Mercuric  sulphofluoride,  2HgS,  HgF2. 

Decomp.  by  boiling  H2O.  Not  decomp.  by 
hot  HC1  or  HNO3+Aq,  but  gives  HF  with 
hot  H2SO4+Aq.  (Rose,  Pogg.  13.  66.) 

Mercury  sulpho'Mmide,  HgN2S,  NH3. 
Ppt.    (Ruff,  B.  1904,  37.  1585.) 

Mercuric  sulphoiodide,  HgS,  HgI2. 
Ppt.    (Rammelsberg,  Pogg.  48.  175.) 
2HgS,  HgI2.    (Palm,  C.  C.  1863.  121.) 


520 


MERCURIC  SULPHOIODIDE  AMMONIA 


Insol.  in  min.  acids  with  exception  of  aqua 
regia.  (Hamers,  Dissert.  1906.) 

Mercuric  sulphoiodide  ammonia,  2HgS, 

Hgli,  NH3. 
(Foerster,  Ch.  Z.  1895,  19.  1895.) 

Mercuric  telluride,  HgTe. 

Min.  ColoradoUe.  Sol.  in  boiling  HNO3  + 
Aq  with  separation  of  H2TeO3. 

Metastannic  acid. 
See  Stannic  acid. 

Molybdatoiodic  acid. 
See  Molybdoiodic  acid. 

Molybdenum,  Mo. 

Not  attacked  by  HC1,  HF,  or  dil.  H2SO4  + 
Aq.  Sol.  in  cone.  H2SO4.  Very  easily  sol.  in 
aqua  regia.  Oxidised  by  HNO3  +  Aq  either  to 
molybdenum  oxide,  which  dissolves  in  HNO3, 
or,  if  HNOs  is  in  excess,  to  molybdic  acid, 
which  remains  undissolved. 

Attacked  by  HNO3+Aq  containing  3-70% 
HNO3,  but  only  slowly  by  70%  acid,  with 
formation  of  insol.  white  powder;  much  more 
vigorously  by  50%  acid,  in  which  case  a  clear 
solution  is  formed.  (Montemartini,  Gazz.  ch. 
it.  22.  384.) 

Not  attacked  by  alkalies -fAq.  (Bucholz, 
Scher.  J.  9.  485.) 

With  a  sp.  gr.  9.01,  the  metal  is  malleable 
and  sol.  in  a  mixture  of  HF  and  HNO3;  sol. 
in  fused  KC1O3.  (Moissan,  Bull.  Soc.  1895, 
(3)  13.  966.) 

Ductile  Mo  is  moderately  quickly  attacked 
by  HNO3,  H2SO4  and  HC1.  (Fink,  Met. 
Chem.  Eng.  1910,  8.  341.) 

Not  immediately  attacked  by  cold  dil. 
HNO3.  Not  attacked  by  dil.  and  cone. 
H2SO4.  Boiling  dil.  HCl+Aq  does  not  at- 
tack; cone,  dissolves  traces  by  long  heating. 
Sol.  in  aqua  regia.  (Lederer,  Dissert.  1911.) 

Dil.  HC1  dissolves  20.3%  Mo  at  110°  in 
18  hrs.  More  slowly  sol.  in  HC1  (sp.  gr. 
1.15). 

Insol.  in  dil.  H2SO4  at  110°.  Slowly  sol. 
in  cone.  H2SO4  (sp.  gr.  1.82)  at  110°,  rapidly 
sol.  at  200°-250°. 

Slowly  sol.  in  cone.  HNO3  (sp.  gr.  1.40), 
rapidly  sol.  in  dil.  HNO3  (sp.  gr.  1.15). 

Rapidly  sol.  in  hot  aqua  regia.  Insol.  in 
hot  or  cold  HF.  (Ruder,  J.  Am.  Chem.  Soc. 
1912,  34.  388.) 

Insol.  in  KOH+Aq.  Sol.  in  fused  KOH. 
(Ruder,  J.  A.m.  Chem.  Soc.  1912,  34.  389.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

Molybdenum  acichloride. 
See  Molybdenyl  chloride. 


Molybdenum  amide,  OH.MoO2.NH2. 

Very  unstable.  Insol.  in  abs.  alcohol. 
(Fleck,  Z.  anorg.  1894,  7.  353.) 

Molybdenum    amide    nitride,    Mo5Ni9H4  = 

4MoN2,  Mo(NH2)2. 

Not  attacked  by  HC1,  or  dil.  HNO3+Aq. 
(Uhrlaub.) 

Molybdenum  amidochloride,  Mo2(NH2)3Cl3. 
Insol.  in  H2O  and  dil.  acids.    (Rosenheim, 
Z.  anorg.  1905,  46.  317.) 

Molybdenum  amidochloride  ammonia, 

Mo2(NH2)3Cl3,  10NH3. 
Unstable  in  the  air.    (Rosenheim,  Z.  anorg. 
1905,  46.  319.) 

Molybdenum  boride,  Mo3B4. 

Moderately  attacked  by  hot  cone,  acids 
and  vigorously  by  hot  aqua  regia.  (Tucker 
and  Moody,  Chem.  Soc.  1902,  81.  17.) 

Molybdenum  <M>romide,  MoBr2  =  Mo3Br4Br2. 
See  Bromomolybdenum  bromide. 

Molybdenum  ^ribromide,  MoBr3. 

Not  decomp.  by  H2O.  Boiling  cone.  HC1, 
and  cold  dil.  HNO3+Aq  do  not  attack  appre- 
ciably. Dil.  alkalies  act  slowly,  but  decomp. 
with  separation  of  Mo2O3  on  boiling.  (Blom- 
strand,  J.  pr.  82.  435.) 

Molybdenum  ^rabromide,  MoBr4. 

Rapidly  deliquescent,  and  easily  sol.  in 
H2O.  (Blomstrand,  J.  pr.  82.  433.) 

Molybdenum  bromochloride,  etc. 
See  Bromomolybdenum  chloride,  etc. 

Molybdenum  bronze. 
See  Molybdate  molybdenum  oxide,  sodium. 

Molybdenum  carbide,  Mo2C. 

Insol.  in  HNO3.  (Moissan,  Bull.  Soc. 
1895,  (3)  13.  967.) 

MoC.  Does  not  decomp.  H2O  even  at 
500-600°.  Slowly  attacked  by  hot  HC1,  HF 
and  hot  cone.  H2SO4.  Easily  decomp.  by 
HNO3.  Not  attacked  by  NaOH+Aq  or 
KOH+Aq.  (Moissan  and  Hoffmann,  C.  R. 
1904,  138.  1559.) 

Molybdenum  carbonyl,  Mo(CO)6. 

Quickly  attacked  by  bromine.  Sol.  in 
ether  or  benzene.  (Mond,  Hirtz  and  Cowap, 
Chem.  Soc.  1910,  97.  808.) 

Molybdenum  ^'chloride,  MoCl2  =  Mo3Cl4Cl2. 
See  Chloromolybdenum  chloride. 


MOLYBDENUM  NITRIDE 


521 


Molybdenum  trichloride,  MoCl3. 

Insol.  in  H2O  or  boiling  cone.  HCl+Aq. 

Easily  sol.,  especially  when  heated,  in  HNO3 

+Aq.    Sol.  in  H2SO4.    Decomp.  by  NH4OH, 

KOH,  orNaOH+Aq. 

SI.  sol.  in  alcohol.    (Leichti  and  Kempe.) 
Practically   insol.    in    alcohol    and    ether. 

(Hampe,  Ch.  Z.  1888,  12.  5.) 

Molybdenum  te/rachloride,  MoCl4. 

Deliquescent.  Hisses  with  little  H2O,  but 
only  partly  sol.  in  more  H2O.  Only  si.  sol.  in 
cone.  HCl+Aq.  Sol.  in  H2S04  or  HNO3  + 
Aq.  Partly  sol.  in  alcohol  and  ether.  (Liechti 
and  Kempe.) 

Molybdenum  perctochloride,  MoCl5. 

Very  deliquescent.  Sol.  in  H2O  with  ex- 
treme evolution  of  heat.  Sol.  in  HC1,  HNO3, 
or  H2SO4+Aq. 

When  freshly  prepared,  is  incompletely  sol. 
in  H2O,  but  after  standing  is  easily  sol.  with 
hissing.  (Kalischer,  Dissert.  1902.) 

Sol.  in  a  small  amt.  of  cone.  HC1.  (Harnpe, 
Ch.  Z.  1888,  12.  5.) 

Sol.  in  absolute  alcohol  or  ether.  (Liechti 
and  Kempe.) 

Sol.  in  CHC13  and  in  CC14.  Sol.  with  hissing 
in  many  organic  solvents  (ethers,  alcohols, 
ketones,  aldehydes,  acids,  acid  esters,  acid 
anhydrides,  amines).  Sol.  in  cinnamic  alde- 
hyde. (Kalischer,  Dissert.  1902.) 

Molybdenum  hydroxyl  chloride,  Mo(OH)2Cl2. 
Easily  sol.  in  H2O.     (Debray,  C.  R.  46. 
1101.) 

Molybdenum  /e/rachloride  phosphorus  penta- 
chloride,  MoCl4,  PC15. 

Sol.  in  H2O. 

MoCl4,  2PC15.  Sol.  in  H2O.  (Cronander, 
Bull.  Soc.  (2)  19.  500.) 

Molybdenum  phosphorus  pe/^achloride, 

MoCl5,  PC15. 

Easily  decomp.  (Smith  and  Sargent,  Z. 
anorg.  1894,  6.  385.) 

Molybdenum    phosphoryl    chloride,    MoCl5, 

POC13. 

Decomp.  by  H2O:  insol.  in  CS2;  sol.  in 
C6H6  and  CHC13. 

Molybdenum  in-chloride  potassium  chloride. 

Efflorescent.  Decomp.  with  H2O.  (Ber- 
zelius.) 

MoCl3,  3KC1.  Very  sol.  in  H2O.  Nearly 
insol.  in  alcohol  and  ether.  (Chilesotti,  C.  C. 
1903,  II.  652.) 

+2H2O.  Fairly  easily  sol.  in  cold  H2O 
without  any  apparent  decomp.  Decomp.  in 
aqueous  solution,  slowly  in  the  cold  but 
rapidly  on  boiling.  This  decomp.  is  pre- 
vented by  the  presence  of  HC1. 


SI.  sol.  in  cone.  HC1.  (Henderson,  Proc. 
Chem.  Soc.  1903,  19.  245.) 

Molybdenum  rubidium  chloride,  Rb2MoCl5 

+H20. 

Sol.  in  H2O.  Nearly  insol.  in  alcohol  and 
ether.  (Chilesotti,  C.  C.  1903,  II.  652.) 

Molybdenum     pentacbloride    nitrogen    sul- 
phide, Mods,  N4S4. 

Decomp.  in  moist  air.  (Davis,  Chem.  Soc. 
1906,  89,  (2)  1575.) 

Molybdenum  Aezafluoride,  MoF6. 

Decomp.  by  a  little  H2O  with  separation 
of  blue  oxide.  Sol.  in  large  amount  of  H2O 
forming  a  colorless  solution. 

Absorbed  by  alkalies  and  NH4OH+Aq. 
(Ruff,  B.  1907,  40.  2930.) 

Molybdenum  fluoride  with  MF. 
See  Fluomolybdate,  M. 

Molybdenum  potassium  ^n'fluoride  (?). 
Precipitate.    Sol.  in  HCl+Aq. 

Molybdenum  potassium  tetr a fluoride  (?). 
SI.  sol.  in  H2O.    (Berzelius.) 

Molybdenum  sesquihydroxide,  Mo2OeH6. 

Difficultly  sol.  in  acids.  Insol.  in  KOH, 
NaOH,  NH4OH,  or  K2CO3+Aq.  Somewhat 
sol.  in  (NH4)2CO3+Aq,  but  pptd.  on  boiling. 
(Berzelius.) 

Molybdenum  hydroxide,  Mo3O8,  5H2O. 

Easily  sol.  in  H2O.  Insol.  in  CaCl2, 
NH4C1,  or  NaCl+Aq.  SI.  sol.  in  alcohol. 
(Berzelius.) 

Molybdenum  d/hydroxide,  MoO2,  zH2O. 

Slowly  and  not  abundantly  sol.  in  H2O, 
from  which  it  is  precipitated  by  NH4C1  and 
other  salts.  Gelatinises  by  standing  in  closed 
vessels  or  by  evaporating  on  the  air.  Sol.  in 
the  ordinary  acids.  Insol.  in  KOH,  or  NaOH 
+Aq.  Sol.  in  alkali  carbonates  -f  Aq. 

Molybdenum  duodide,  MoI2. 

Insol.  in  H2O  and  alcohol.  SI.  attacked 
by  cold  H2SO4  or  HNO3.  (Guichard,  A. 
ch.  1901,  (7)23.567.) 

SI.  deeomp.  H2O  at  ordinary  temp.  Slowly 
sol.  in  H2SO4  and  HNO3.  (Guichard,  C.  R. 
1896,  123.  822.) 

Molybdenum  tetraiodide  (?). 
Completely  sol.  in  water.    (Berzelius.) 

Molybdenum  nitride,  Mo5N3,  and  Mo5N4. 

(Uhrlaub.) 

See  Molybdenum  amide. 

Mo3N2.  (Rosenheim,  Z.  anorg.  1905,  46. 
317.) 


522 


MOLYBDENUM  OXIDE 


Molybdenum  monoxide,  MoO. 

Known  only  as  hydroxide.  (Blomstrand,  J. 
pr.  77.  90.) 

Molybdenum  sesq Dioxide,  Mo2O3. 
Insol.  in  acids  or  alkalies. 
See  Molybdenum  sesginhydroxide. 

Molybdenum  efroxide,  MoO2. 

Insol.  in  HC1  or  HF+Aq.  SI.  sol.  in  cone. 
H2SO4.  HNO3  oxidises  to  MoO3.  Not  at- 
tacked by  KOH+Aq.  (Ullik,  A.  144.  227.) 

SI.  sol.  in  KHC4H4O6+Aq. 

Molybdenum  /noxide,  MoO3. 

Sol.  in  500  pts.  cold,  and  much  less  hot  H2O. 
(Bucholz.) 

Sol.  in  960  pts.  hot  H2O.    (Hatchett.) 

Sol.  in  570  pts.  cold,  and  much  less  hot  H2O. 
(Dumas.) 

Sol.  in  acids  before  ignition.  Insol.  in  acids, 
but  si.  sol.  in  acid  potassium  tartrate+Aq 
after  ignition.  Sol.  in  alkalies  or  alkali  car- 
bonates +Aq. 

Sol.  in  NH4OH+Aq. 

See  also  Molybdic  acid. 

Min.  Molybdite.    Sol.  in  HCl+Aq. 

Molybdenum  oxide,  Mo2O5. 

Sol.  in  H2SO4  and  HC1;  only  si.  sol.  in 
H2SO4.  (Klason,  B.  1901,  34.  151.) 

+3H2O.  SI.  sol.  in  H2O  (2  g.  in  1  1.). 
Insol.  in  NH4Cl+Aq.  Insol.  in  caustic  al- 
kalies, somewhat  sol.  in  NH4OH.  Much 
more  sol.  in  M2CO3+Aq  and  in  (NH4)2CO3  + 
Aq.  (Klason,  B.  1901,  34.  150.) 

Mo4Oio+3H2O.  (Smith  and  Oberholtzer, 
Z.  anorg.  1893,  4.  243.) 

Mo4On+6H2O.  Sol.  inH2O.  (Bailhache, 
C.  R.  1901,  133.  1212.) 

MoftO34+6H2O.  Very  sol.  in  H2O.  (Guich- 
ard,  C.  R.  1900,  131.  419.) 

Mo7O20.  Sol.  in  H2O.  (Junius,  Z.  anorg. 
1905,  46.  447.) 

Mo20O41+2lH2O  =  Mo2O5,  18MoO2  + 
21H2O.    Easily  sol.  in  H2O.    Insol.  in  NH4C1 
+Aq.    (Klason,  B.  1901,  34.  160.) 

Mo26O77+24H2O  =  Mo2O5,  24MoO3-f 
24H2O.    (Klason,  B.  1901,  34.  159.) 

3Mo2O3,  2Mo7O24  +  18H2O.  Sol.  in  H2O. 
(B.) 

It  is  probable  that  the  five  blue  oxides  of 
molybdenum  described  by  Klason  (B.  34, 
148.  158)  and  Bailhache  are  either  the  blue 
oxide  Mo5Ou  prepared  by  the  author  or  mix- 
tures of  this  compd.  with  molybdenum  tri- 
oxide.  (Guichard,  C.  R.  1902, 134. 173.) 

Mo5O12.  Not  attacked  by  ammonia;  easily 
oxidised  by  HNO3+Aq.  Not  attacked  by 
HC1  or  H2SO4+Aq.  (Wohler,  A.  110.  275.) 

Formula  is  Mo3O8,  according  to  Wohler, 
but  Muthmann  (A.  238.  108)  has  shown  that 
correct  formula  is  Mo6Oj2. 

Not  attacked  by  boiling  alkalies,  HC1,  or 
dil.  H2SO4+Aq.  Sol.  in  cone.  H2SO4,  with 


subsequent  decomp.  Sol.  in  aqua  regia,  and 
Cl2+Aq.  (Muthmann.) 

Mo3O8.  Sol.  in  H2O.  (Muthmann,  A. 
238.  108.) 

Min.  Ilsemannite  (?). 

+5H2O.  Moderately  sol.  in  H2O.  (Mar- 
chetti,  Z.  anorg.  1899,  19.  393.) 

Mo5O7.    (v.  d.  Pfordten,  B.  16.  1925.) 

Molybdenum  tr  /oxide  ammonia,  MoO3, 3NH3. 

Unstable  in  air.  Very  sol.  in  H2O  with 
evolution  of  ammonia.  (Rosenheim,  Z. 
anorg.  1906,  50.  303.) 

3MoO3,  NH3  +  i^H2O.  True  composition 
of  commercial  molybdic  acid.  (Klason,  B. 
1901,  34.  156.) 

NH4H3MosOi2.  Very  si.  sol.  in  cold,  easily 
sol.  in  hot  H2O  with  partial  decomp.  (Klason, 
B.  1901,  34.  156.) 

3MoO3,  3NH3+7H2O  =  (NH4)3H3Mo3Ols 
+4H2O.  True  composition  of  Rammelsberg's 
3(NH4)2O,  7MoO3+12H2O.  (Klason,  B. 
1901,  34.  155.)  ' 

4MoO3,  NH3+6H2O.  Very  si.  sol.  in  cold, 
very  easily  sol.  in  hot  H2O.  An  insol.  modi- 
fication with  less  H2O  gradually  cryst.  out. 
(Mylius,  B.  1903,  36.  639.) 

4MoO3,  2NH3+3H2O.  (Klason,  B.  1901, 
34.  156.) 

6MoO3,  3NH3+5H2O.  Very  si.  sol.  in 
cold,  more  easily  sol.  in  hot  H20,  with  partial 
decomp.  (Klason,  B.  1901,  34.  156.) 

12MoO3,  3NH3  +  12H2O.  (Klason,  B. 
1901,  34.  158.) 

12MoO3,  3NH3,  12H2O+3MoO3,  8H2O. 
Moderately  sol.  in  boiling  H2O.  (Klason.) 

15MoO3,  3NH3+6H2O.  Insol.  in  H2O. 
(Klason.) 

4MoO3,  MoO2,  2NH3+7H2O.  Slowly  sol. 
in  H2O;  fairly  stable,  gradually  decomp.  by 
dil.  acids.  (Hofmann,  Z.  anorg.  1896,  12. 
280.) 

Molybdenum    ^n'oxide    ammonia    hydrogen 
peroxide,     18MoO3,     14NH3,     3H2O2  + 
18H20. 
Sol.  in  H2O.     Sp.  gr.   of  sat.  solution  = 

1.486  at  17.4°.    (Baerwald,  B.  1884, 17. 1206.) 

Molybdenum  oxybromide. 
See  Molybdenyl  bromide. 

Molybdenum  oxychloride. 
See  Molybdenyl  chloride. 

Molybdenum  oxyfluoride. 
See  Molybdenyl  fluoride. 

Molybdenum  oxyfluoride  with  MF. 

See  Fluoxymolybdate,  M,  and  Fluoxyhypo- 
molybdate,  M. 

Molybdenum  phosphide,  Mo2P2. 

Gradually  sol.  in  hot  HNO3+Aq.  (Wohler 
and  Rautenberg,  A.  109.  374.) 


MOLYBDENYL  RUBIDIUM  CHLORIDE 


523 


Molybdenum  selenide,  MoSe3. 

Not  obtained  pure.  (Uelsmann,  A.  116. 
125.) 

Molybdenum  silicide. 

Sol.  in  HF;  only  very  si.  sol.  in  other  acids. 
(Warren,  C.  N.  1898,  78.  319.) 

MoSi2.  Insol.  in  all  min.  acids;  sol.  in  a 
warm  mixture  of  HF+HNO3.  (Defacqz, 
C.  R.  1907,  144.  1425.) 

Insol.  in  min.  acids;  sol.  in  HF+HNO3. 
Unattacked  by  10-20%  KOH+Aq.  De- 
comp.  by  fused  NaOH.  (Honigschmid,  M. 
1907,  28.  1020.) 

Not  attacked  by  boiling  HNO3,  aqua  regia 
or  HF.  (Watts,  Trans.  Am.  Electrochem. 
Soc.  1906,  9.  106.) 

Mo2Sis.    (Vigouroux,  C.  R.  129.  1238.) 

Molybdenum  ^sulphide,  MoS2. 

Insol.  in  H2O.  Easily  sol.  in  aqua  regia. 
Easily  oxidised  by  HNO3.  Sol.  in  boiling 
H2SO4.  SI.  attacked  by  KOH+Aq.  (Ber- 
zelius.) 

Min.  Molybdenite.  Sol.  in  HNO3+Aq, 
with  separation  of  MoO3;  sol.  in  aqua  regia; 
very  si.  sol.  in  H2SO4. 

Molybdenum  irisulphide,  MoS3. 

Somewhat  sol.  in  H2O,  especially  if  hot,  but 
pptd.  by  an  acid.  Difficultly  sol.  except  when 
boiled  with  KOH+Aq.  SI.  sol.  in  solutions 
of  alkali  sulphides  unless  heated.  (Berzelius.) 

Easily  sol.  in  alkali  sulphides +Aq;  slowly 
sol.  in  alkalies  or  alkali  hydrosulphides+Aq. 
(Atterberg,  J.  B.  1873.  258.) 

Molybdenum  tefrasulphide,  MoS4. 

Not  decomp.  by  hot  H2O  or  acids. 

SI.  sol.  in  cold  alkali  sulphides +Aq,  but 
easily  by  boiling.  (Berzelius.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 

Molybdenum  sesg?«'sulphide,  Mo2S3. 

Insol.  in  HC1  and  H2SO4;  sol.  in  hot  cone. 
HNO3  and  aqua  regia.  (Guichard,  C.  R. 
1900,  130.  138.) 

Molybdenum  sulphide  with  MS. 
See  Sulphomolybdate,  M. 

Molybenum  sulphochloride,  Mo5S8Cl9. 

Insol.  in  H2O  and  alkalies.  Slowly  sol.  in 
cone.  HNO3.  (Smith  and  Oberholtzer,  Z. 
anorg.  1894,  5.  67.) 


Molybdenyl  monamide,  NH4MoO4  or 

Mo°<NH2+H'°- 
(Rosenheim,  Z.  anorg.  1905,  46.  318.) 


Molybdenyl  bromide,  MoO2Br2. 

Deliquescent,  and  sol.  in  H2O  with  slight 
evolution  of  heat. 

Mo2O3Br4.  Unstable  in  air.  (Smith  and 
Oberholtzer,  Z.  anorg.  4.  236.) 

Molybdenyl    potassium   bromide,    MoOBr3, 

2KBr. 

(Weinland,  Z.  anorg.  1905,  44.  109.) 
MoOBr3,     KBr+2H2O.       (Weinland,     Z. 

anorg.  1905,  44.  110.) 

Molybdenyl    rubidium    bromide,    MoOBr3, 

2RbBr. 
(Weinland,  Z.  anorg.  1905,  44.  108.) 

Molydenyl  chloride,  MoO2Cl2. 

Sol.  in  H2O  and  alcohol. 

Abundantly  sol.  in  abs.  alcohol.  Not  very 
sol.  in  abs.  ether.  (Hampe,  Ch.  Z.  1888,  12. 
23.) 

+H2O.  Composition  settled  by  mol.  wt. 
determinations.  Dissociates  in  alcohol  and 
in  H2O.  (Vaudenberghe,  Z.  anorg.  1895,  10. 
52.) 

Very  hygroscopic.  Sol.  in  acetone,  ether 
and  alcohol.  (Vaudenberghe,  I.  c.) 

MoOCl4.  Deliquescent.  Sol.  in  little  H2O 
with  violent  action.  More  H2O  decomposes. 
(Puttbach,  A.  201.  123.) 

Formula  is  Mo9O8Cl32,  according  to  Blom- 
strand  (J.  pr.  71.  460). 

Mo2O3Cl4.    (Puttbach,  I.  c.) 

Mo2O3Cl6.  Deliquescent.  Sol.  in  H2O  with 
very  slight  evolution  of  heat  and  subsequent 
formation  of  precipitate.  (Blomstrand.) 

Sol.  in  acids.    (Puttbach,  A.  201.  129.) 

Mo2O3Cl5.  Deliquescent,  and  sol.  in  H2O. 
(Blomstrand.) 

Mo3O5Cl8.  Insol.  in  HC1  and  cold  H2SO4. 
Sol.  in  hot  H2SO4  and  HNO3.  (Puttbach,  A. 
201.  123.) 

Mo3O3Cl7.  Difficultly  sol.  in  HC1.  Easily 
sol.  in  HNO3,  and  alkalies +Aq.  (Puttbach.) 

Molybdenyl  potassium  chloride,  MoO2Cl2, 
KC1+H2O. 

(Weinland,  Z.  anorg.  1905,  44.  97.) 

+2H2O.  (Weinland,  Z.  anorg.  1905,  44. 
96.) 

6MoO2Cl2,  2KC1+6H2O.  (Weinland,  Z. 
anorg.  1905,  44.  97.) 

MoOCl3,2KCl+2H2O.  Sol.inH2O.  (Nor- 
denskjold,  B.  1901,  34.  1573.) 

Ppt.  (Henderson,  Proc.  Chem.  Soc.  1903, 
19.245.) 

Molybdenyl  rubidium  chloride,  MoO2Cl2, 
RbCl+H2O. 

MoO2Cl2,  2RbCl.  (Weinland,  Z.  anorg. 
1905,  44.  95.) 

MoOCl3,  2RbCl.  SI.  sol.  in  H2O.  Less  sol. 
than  K  salt.  (Nordenskjold,  B.  1901,  34. 
1573.) 


524 


MOLYBDENYL  FLUORIDE 


Molybdenyl  fluoride,  MoO2F2. 

Decomp.  rapidly  in  moist  air.  (Schulze,  J. 
pr.  (2)  21.  442.) 

Very  hydroscopic.  Sol.  in  a  little  H2O  giv- 
ing a  blue  solution;  in  more  H2O  giving  a 
colorless  solution. 

Sol.  in  AsCl3,  SiCl4,  SO2C12  and  PC13.  On 
warming  these  solutions,  gas  is  evolved. 

Insol.  in  toluene.  Nearly  insol.  in  ether, 
CHC13,  CC14,  and  CS2.  Sol.'in  warm  pyridine 
and  in  ethyl  and  methyl  alcohol.  (Ruff,  B. 
1907,  40.  2934.) 

MoOF4.  Very  hydroscopic.  Decomp.  by 
H2O  and  cone.  H2SO4.  Decomp.  by  alcohol. 
Sol.  in  ether  and  CHC13  with  evolution  of  gas. 
Insol.  in  toluene.  Very  si.  sol.  in  benzene 
and  CS2.  (Ruff,  B.  1907,  40.  2932.) 

Mo2O3F4.  Deliquescent.  Easily  sol.  in  HF 
+Aq,  not  ^n  H2O.  (Smith  and  Oberholtzer.) 

Molybdenyl  fluoride  with  MF. 

See  Fluoxymolybdate,  M,  and  Fluoxyhypo- 
molybdate,  M. 

Molybdenyl  hydroxide,  MoO(OH)3. 

2  g.  are  sol.  in  1000  cc.  H2O;  insol.  in  H2O  + 
NH4C1;  only  si.  sol.  in  NH4OH  and  alkali 
carbonates +Aq.  (Klason,  B.  1901,  34.  151.) 

Molybdic  acid,  H2MoO4. 

(Ullik,  A.  144.  217.) 

Nearly  insol.  in  H20.  (Vivier,  C.  R.  106. 
601.) 

Very  sparingly  sol.  in  cold  H2O,  more  sol. 
in  hot  H2O.  (Rosenheim  and  Bertheim,  Z. 
anorg.  1903,  34.  435.) 

a-modification. 

Solubility  of  MoO3,  H2O  (a-modification)  in 

H2O  at  t°. 
1000  g.  H2O  dissolve  g.  Mo03. 


(Rosenheim  and  Davidsohn,  Z.  anorg.  1903, 
37.  318.) 

(j8  modification),  MoO3,  H2O.  From 
MoO3,  2H2O  at  60°-70°.  (Rosenheim  and 
Davidsohn.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

Easily  sol.  in  H2SO4.  (Ruegenberg  and 
Smith,  J.  Am.  Chem.  Soc.  1900,  22.  772.) 

H4MoO5.  Sol.  in  H2O  and  acids.  (Mil- 
lingk.) 


t° 

G.  MoO3 

"  t 

G.  MoO3 

18 

1.066 

59 

11.258 

23 

1.856 

60 

12.057 

30 

2.638 

66 

17.274 

40 

4.761 

70 

20.550 

48 

6.360 

74.4 

20.904 

50.2 

6.873 

75 

20.920 

54 

•    7.855 

79 

21.064 

Solvent 

t° 

G.  Mo03 

10%  (NH4)2S04 

10%  NH4HSO4 

a 

(C 

29.6 
31.5 
41.8 
49.7 

19.27 
27.53 
34.36 
37.69 

t° 

G.  Mo03 

t° 

G.  Mo03 

14.8 

2.117 

42.0 

3.446 

15.2 

2.131 

45.0 

3.661 

24.6 

2.619 

52.0 

4.184 

25.6 

2.689 

60.0 

4.685 

30.3 

2.973 

70.0 

4.231 

36.0 

3.085 

80.0 

5.212 

36.8 

3.295 

Very  sol.  in  H2O.     (Mylius,  B.  1903,  36, 
638.) 

Solubility  of  MoO3,  2H2O  in  H2O. 
1000  g.  H2O  dissolve  g.  MoO3  at  t°. 


(Rosenheim  and  Bertheim,  Z.  anorg.  1903,  34. 
430.) 

Solubility  of  MoO3,  2H2O  in  ammonium  salts 

+Aq  at  t°. 
1000  g.  of  the  solvent  dissolve  g.  MoO3. 


(Rosenheim  and  Davidsohn,  Z.  anorg.  1903, 
37.  315.) 

H6MoOfl  (?).    Known  only  in  solution. 
H2Mo2O7.    Easily  sol.  in  H2O.    (Ullik.) 
H2Mo4O13.      Easily    sol.    in    H2O.      (U.) 
H2Mo8O25.    Easily  sol.  in  H2O.     (U.) 
Molybdic  acid  also  exists  in  a  colloidal 

modification,  sol.  in  H2O.     (Graham,  C.  R. 

69.  174.) 

Molybdates. 

The  normal  molybdates  of  the  alkali  metals 
are  easily  sol.  in  H2O,  while  the  others  are 
si.  sol.  or  insol.  therein. 

The  frimolybdates  are  si.  sol.  in  cold,  but 
very  easily  sol.  in  hot  H2O. 

The  tetramolybdates  are  easily  sol.  in  H2O. 

Aluminum  molybdate,  Ali0Mo2O2i. 
Precipitate.    (Gentele,  J.  pr.  81.  414.) 
Contains    aluminum    hydroxide    and    sul- 
phate.   (Struve,  J.  pr.  61.  441.) 

Aluminum  ammonium  molybdate. 
See  Aluminicomolybdate,  ammonium. 

Aluminum  barium  molybdate. 
See  Aluminicomolybdate,  barium. 

Ammonium   molybdate,    (NH4)2MoO4. 

Efflorescent  through  loss  of  NH3;  decomp. 
by  H2O  into  acid  salt.  (Svanberg  and  Struve.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  826.) 


MOLYBDATE,  AMMONIUM  MANGANOUS 


525 


(NH4)2Mo2O7.    Sol.  in  H2O. 

+H2O  =  NH4HMoO4.  Sol.  in  H2O.  Sol. 
in  2-3  pts.  H2O.  (Brandes;  Mauro,  Gazz. 
ch.  it.  18.  120.) 

(NH4)6Mo7O24+4H2O.  (Commercial  am- 
monium molybdate.) 

Not  efflorescent.  Sol.  in  H2O.  (Delafon- 
taine,  N.  Arch.  Sc.  ph.  nat.  23.  17.) 

According    to    Struve    and    Berlin  = 
(NH4)4Mo6O17+3H2O. 

According  to  Marignac  and  Delffs  = 
(NH4)HMoO4.      The    true    composition    of 
commercial    ammonium    molybdate    is 
(NH4)i0Moi2O4i.      (Junius,   Z.   anorg.    1905, 
46.  428.) 

+  12H2O.  More  sol.  than  the  above. 
(Rammelsberg,  Pogg.  127.  298.) 

Insol.  in  acetone.  (Krug  and  M'Elroy,  J. 
Anal.  Appl.  Ch.  6.  184.) 

(NH4)ioMoi2O4i.  True  formula  for  com- 
mercial ammonium  molybdate  (Sand  and 
Eisenlohr,  Z.  anorg.  1907,  52.  68.) 

+7H2O.    (Junius,  Z.  anorg.  1905,  46.  428.) 

(NH4)4Mo6Oi7+H2O.  (Jean,  C.  R.  78. 
436.) 

(NH4)2Mo2O19+H2O.  Very  difficultly  sol. 
in  cold,  easily  sol.  in  hot  H2O.  (Berlin,  J.  pr. 
49.  445.) 

Easily  sol.  in  NH4OH+Aq.  (Kammerer, 
J.  pr.  (2)  6.  358.) 

(NH4)2O,  4MoO3.  Practically  insol.  in 
cold,  si.  sol.  in  hot  H2O.  (Westphal,  Dissert. 
1995.) 

+2H2O.  Very  difficultly  sol.  in  cold, 
rather  easily  sol.  in  hot  H2O.  (Berlin.) 

100  cc.  H2O  dissolve  3.5200  g.  at  15°;  sp. 
gr.  =  1.03;  3.6711  g.  at  18°;  sp.  gr.  =  1.04; 
4.5961  g.  at  32°;  sp.  gr.  =  1.05.  (Wempe,  Z. 
anorg.  1912,  78.  258.) 

+2^H2O.  (Junius,  Z.  anorg.  1905,  46. 
440.) 

(NH4)2O,  8MoO3+13H2O.  (Rosenheim, 
Z.  anorg.  1897,  15.  188.) 

(NH4)oO,  9MoO3  +  17H2O.  (Westphal, 
Dissert.  1895.) 

See  also  Molybdenum  /rioxide  ammonia. 

Ammonium  barium  molybdate, 

3(NH4)2O,    3BaO,     14MoO3  +  12H2O. 
(Westphal,  Dissert.  1895.) 

Ammonium   bismuth  molybdate, 

NH4Bi(MoO4)2. 

(Riederer,  J.  Am.  Chem.  Soc.  1903,  25. 
914.) 

Ammonium  cadmium  molybdate   ammonia, 

(NH4)2Cd(MoO4)2,  2NH3. 
Decomp.  by  H2O. 

Sol.  in  dil.  NH4OH+Aq.  (Briggs,  Chem. 
Soc.  1904,  85.  674.) 

Ammonium  cerium  molybdate, 
(NH4)6CeMo14O48+24H2O. 
Sol.  in  H2O.    (Barbieri,  C.  A.  1909.  293.) 


Ammonium  chromic  molybdate. 

See  Chromicomolybdate,  ammonium. 

Ammonium  cobaltous  molybdate, 

3(NH4)2O,  7MoO3,  3CoO,  7MoO3+*H2O. 

5[3(NH4)2O,  7MoO3],  7[3CoO,  7MoO3]  + 
zH2O. 

2[3(NH4)oO,  7MoO3],  3[3CoO,  7MoO3j 
+xH20. 

3[3(NH4)2O,  7MoO3],  5[3CoO,  7MoO3] 
+xR2O. 

3(NH4)2O,     7MoO3,     5[3CoO,     7MoO3]  + 


9[2(NH4)2O,  5MoO3],  5[2CoO,  5MoO3]  + 
118  H2O. 

4(NH4)2O,  2CoO,  15MoO3+20H2O. 
(Marckwald,  Dissert.  1895.) 

Ammonium  cobaltous  molybdate  ammonia, 

(NH4)2Co(MoO4)2,  2NH3. 
Decomp.  by  H2O. 

Sol.  in  dil.  NH4OH+Aq.  (Briggs,  Chem. 
Soc.  1904,  85.  674.) 

Ammonium  cobaltic  molybdate. 
See  Cobaltimolybdate,  ammonium. 

Ammonium  cupric  molybdate,  (NH4)2O,  CuO, 

5MoO3+9H2O. 

SI.  sol.  in  cold,  sol.  in  boiling  H2O  without 
decomp.  (Struve.) 

Ammonium  cupric  molybdate  ammonia, 
(NH4)2Cu(MoO4)2,  2NH3. 

Sol.  in  dil.  NH4OH+Aq. 

Decomp.  by  H2O.  (Briggs,  Chem.  Soc. 
1904,  85.  673.) 

Ammonium  ferric  molybdate,  3(NH4)2Mo2O7> 

Fe2(MoO4)6+20H2O. 
Sol.  in  H2O.  (Struve.) 
See  also  Ferricomolybdate,  ammonium. 

Ammonium  lanthanum  molybdate, 

(NH4)6La2Mo14O48+24H2O. 
Sol.  in  H2O.    (Barbieri,  C.  A.  1909.  293.) 

Ammonium  lithium  molybdate,  NH4LiMoO4 

+H20. 
(Traube,  N.  Jahrb.  Miner.  1894,  I.  194.) 

Ammonium  magnesium  molybdate,  (NH4)2(X 
MgO,  2MoO3+2H2O  =  (NH4)2MoO4, 
MgMoO4+2H2O. 
Easily  sol.  in  H2O.     (Ullik,  A.  144.  344.) 

Ammonium  manganous  molybdate, 
2(NH4)20,  MnO,  3MoO3+5H2O. 

Decomp.  by  boiling  H2O.  (Marckwald, 
Dissert.  1895.) 

(NH4)2O,  2MnO,  6MoO3+16H2O.  De- 
comp. by  boiling  H2O.  (Marckwald.  Dissert. 
1895.)  ' 


526 


MOLYBDATE,  AMMONIUM  MANGANIC 


(NH4)2O,  3MnO,  6MoO3+16H2O.  De- 
comp.  by  boiling  H2O.  (Marckwald,  Dissert. 
1896.) 

3(NH4)2O,    2MnO,    12MoO3+22H2O. 
(Marckwald,  Dissert.  1895.) 

Ammonium  manganic  molybdate. 

See  Permanganomolybdate  ammonium. 

Ammonium  mercuric  molybdate. 

Sol.  in  HCl+Aq.  Sol.  in  boiling  NH4C1+ 
Aq,  separating  out  on  cooling.  Sol.  in  hot 
(NH4)2SO3+Aq.  (Hirzel.) 

Ammonium  molybdenum  molybdate, 

(NH4)2O,  2MoO2,  4MoO3-f  9H2O. 
Easily  sol.  in  H2O,  but  the  solution  soon 
becomes  cloudy.     (Rammelsberg,  Pogg.  127. 
291.) 

Ammonium  neodymium  molybdate, 

(NH4)  3NdMoO24  +  12H2O. 
Ppf.     (Barbieri,  C.  C.  1911,  I.  1043.) 

Ammonium  nickel  molybdate, 

(NH4)2O,  3NiO,  9MoO3+25H2O. 

Very  si.  sol.  in  cold,  sol.  in  hot  H2O  with- 
out decomp.  (Marckwald,  Dissert.  1895.) 

3(NH4)2O,  2NiO,  10MoO3+14H2O.  Very 
si.  sol.  in  cold,  sol.  in  hot  H2O  without  de- 
comp. (Marckwald,  Dissert.  1895.) 

5(NH4)2O,  3NiO,  16MoO3  +  16H2O.  (Hall, 
J.  Am.  Chem.  Soc.  1907,  29,  702.) 

6(NH4)2O,  3NiO,  16MoO3+29H2O.  Very 
si.  sol.  in  cold,  sol.  in  hot  H2O  without  de- 
comp. (Marckwald,  Dissert.  1895.) 

8(NH4)2O,  6NiO,  31MoO3+63H2O.  Very 
si.  sol.  in  cold,  sol.  in  hot  H2O  without  de- 
comp. (Marckwald,  Dissert.  1895.) 

3(NH4)2O,  9NiO,  34MoO3+120H2O.  Very 
si.  sol.  in  cold,  easily  sol.  in  hot  H2O  without 
decomp.  (Marckwald,  Dissert.  1895.) 

Ammonium  nickelic  molybdate. 
See  Nickelimolybdate,  ammonium. 

Ammonium  nickel  hydrogen  molybdate, 

(NH4)4H6[Ni(MoO4)6]+5H2O. 
See  Nickelomolybdate,  ammonium  hydro- 
gen. 

Ammonium   praseodymium   molybdate, 

(NH4)3PrMoO24  +  12H2O. 
Ppt.    (Barbieri,  C.  A.  1911.  1884.) 

Ammonium  samarium  molybdate, 

(NH4)3SmMoO24  +  12H2O. 
Ppt.    (Barbieri,  C.  A.  1911.  1884.) 

Ammonium  sodium  molybdate,  7(NH4)2O, 
2Na2O,  21MoO3  +  15H2O  (?). 

Easily  sol.  in  H2O.  (Delafontaine,  J.  pr. 
95.  136.) 

7(NH4)2O,  3Na2O,  25MoO3+30H2O  (?). 
(Delafontaine.) 


(NH4,  Na)2O,  3MoO3+H2O.  Sol.  in  H2O. 
(Mauro,  Gazz.  ch.  it.  11.  214.) 

Ammonium  thorium  molybdate. 
See  Thoromolybdate,  ammonium. 

Ammonium  titanium  molybdate. 
See  Titanomolybdate,  ammonium. 

Ammonium  vanadium  molybdate. 
See  Vanadiomolybdate,  ammonium. 

Ammonium  zinc  molybdate. 
Sol.  in  H2O.    (Berzelius.) 

Ammonium  zirconium  molybdate. 
See  Zirconomolybdate,  ammonium. 

Ammonium    molybdate    hydrogen    rfzoxide, 

18Mo03,    7(NH4)20,    3H202  +  11H20. 
Sol.  in  H2O.    (Barwald,  B.  17.  1206.) 

Barium   molybdate,   basic,   2BaO,    MoO3  + 

H20  (?). 

Insol.  in  H2O.  Sol.  in  dil.  HCl+Aq  or 
HNO3+Aq.  (Heine,  J.  pr.  9.  204.) 

Barium  molybdate,  BaMoO4. 

Difficultly  sol.  in  H2O;  sol.  in  dil.  HC1,  and 
HNO3+Aq.  (Svanberg  and  Struve.) 

Sol.  in  17,200  pts.  H2O  at  23°.  More  sol.  in 
NH4NO3+Aq  than  in  H,O.  (Smith  and 
Bradbury,  B.  24.  2930.) 

+3H2O.    (Westphal,  Dissert.  1895.) 

BaMo3O19+3H20.    SI.  sol.  in  H2O. 

Ba3MoO24+9H2O.  Appreciably  sol.  in 
H2O.  (Jorgensen.) 

According  to  Svanberg  and  Struve  = 
Ba2Mo6Oi  +6H2O. 

+  12H2O  or  5BaO,  12MoO3+20H2O. 
(Junius,  Z.  anorg.  1905,  46.  433.) 

+22H2O.      Ppt.      (Westphal,    Dissert. 
1895.) 

BaO,  4MoO3+3^H2O.  Ppt.  (Wempe.  Z. 
anorg.  1912,  78.  320.) 

+12H2O.  Ppt.  (Rosenheim,  Z.  anorg. 
1913,  79.  299.) 

BaMo9O28+4H2O.  Insol.  in  cold  or  hot 
H2O  or  HNO3+Aq.  Extremely  slightly  de- 
comp. by  H2SO4,  or  H2SO4+HNO3,  or  HC1+ 
Aq.  (Svanberg  and  Struve.) 

Barium    paramolybdate,    5BaO,    12MoO3+ 
10H2O. 

Ppt.  Sol.  in  excess  of  BaCl2+Aq.  (Junius, 
Z.  anorg.  1905,  46.  433.) 

Barium     te^amolybdate,     BaH2(Mo4Oj3)2  + 
17H2O. 

Insol.  in  cold,  apparently  decomp.  by  hot 
H2O,  a  small  part  dissolving,  and  the  rest 
forming  an  insol.  residue.  (Ullik,  A.  144. 
336.) 


MOLYBDATE,  COBALTOUS  SODIUM 


527 


+14H2O.  Insol.  in  cold  and  hot  H2O. 
(Wempe,  Z.  anorg.  1912,  78.  320.) 

BaO,  8Mo03+17H2O.  (Felix,  Dissert. 
1912.) 

Barium  chromic  molybdate. 

See  Chromicomolybdate,  barium. 

Barium  cobaltic  molybdate. 
See  Cobaltimolybdate,  barium. 

Barium  manganic  molybdate. 

See  Permanganomolybdate,  barium. 

Barium  nickelic  molybdate. 
See  Nickelimolybdate,  barium. 

Barium  nickel  hydrogen  molybdate, 

Ba2H6[Ni(MoO4)6]  +  10H2O. 
See  Nickelomolybdate,  barium  hydrogen. 

Barium  vanadium  molybdate. 
See  Vanadiomolybdate,  barium. 

Barium  molybdate  hydrogen  dioxide,  8BaO, 

19MoO3,2H2O2  +  13H2O. 
Precipitate.     (Barwald.) 

Bismuth  molybdate,  Bi2O3,  3MoO3. 

Somewhat  sol.  in  H2O.  Sol.  in  500  pts. 
H2O  and  in  the  stronger  acids.  (Richter.) 

Bromomolybdenum  molybdate. 

See  under  Bromomolybdenum  comps. 

Cadmium  molybdate,  CdMoO4. 

Insol.  in  H2O;  sol.  in  NH4OH+Aq,  KCN+ 
Aq,  or  acids.  (Smith  and  Bradbury,  B.  24. 
2390.) 

CdO,  H2O,  8MoO3+6H2O.  Decomp.  by 
boiling  with  H2O.  (Wempe,  Z.  anorg.  1912, 
78.  323.) 

Caesium  molybdate,  Cs2O,  3MoO3+H2O. 

(Ephraim  and  Herschfinkel,  Z.  anorg. 
1909,  64.  270.) 

Cs20,  5Mo03+3H2O.  (Ephraim  and 
Herschfinkel,  Z.  anorg.  1909,  64.  270.) 

+3J^H2O.  Very  si.  sol.  in  cold,  easily  sol. 
in  hot  H2O.  (Wempe,  Dissert.  1911.) 

2Cs2O,  5MoO3+5H2O.  (Ephraim  and 
Herschfinkel,  Z.  anorg.  1909,  64.  271.) 

3Cs2O,  10MoO3+3H2O.  (Ephraim  and 
Herschfinkel,  Z.  anorg.  1909,  64.  271.) 

Cs2O,  16MoO3+8H2O.  (Ephraim  and 
Herschfinkel,  Z.  anorg.  1909,  64.  271.) 

3Cs2O,  10MoO3+3H2O.  (Ephraim  and 
Herschfinkel,  Z.  anorg.  1909,  64.  271.) 

Caesium  teJramolybdate,  Cs2O,  4MoO3. 

Only  si.  sol.  in  H2O.  (Muthmann,  B. 
1898,  31.  1841.) 

+2H2O.  SI.  sol.  in  H2O.  (Muthmann, 
B.  1898,  31.  1841.) 


+3H2O.  Easily  sol.  in  cold  or  hot  F2O. 
(Wempe,  Z.  anorg.  1912,  78.  317.) 

+5H2O.  Very  sol.  in  cold  and  hot  H2O. 
(Wempe,  Dissert.  1911.) 

Cs2O,  MoO3,  Cs2O,  3MoO3+4.5H2O.  Sol. 
in  H2O.  (Wempe,  Z.  anorg.  1912,  78.  317.) 

Caesium  paramolybdate,   5Cs2O,    12MoO3-f 
11H2O. 

Efflorescent.  Easily  sol.  in  H2O.  (Wempe, 
Z.  anorg.  1912,  78.  317.) 

Calcium  molybdate,  CaMoO4. 

Insol.  precipitate.    (Ullik.) 

SI.  sol.  in  H2O;  insol.  in  alcohol.  (Smith 
and  Bradbury,  B.  24.  2930.) 

+H2O.     (Westphal,  Dissert.  1896.) 

+2H2O.     (Westphal,   Dissert.  1895.) 

+6H2O.  Difficultly  sol.  in  cold,  easily  in 
hot  H2O.  (Ullik,  A.  144.  231.) 

CaMo4O13+9H2O.    Easily  sol.  in  cold  H2O. 

CaO,  2H2O,  12MoO3+21H2O.  Efflores- 
cent. SI.  sol.  in  cold,  easily  sol.  in  hot  H2O. 
(Wempe.) 

Calcium  hydrogen  teiramolybdate, 
CaH2(Mo4O13)2+17H2O. 

SI.  sol.  in  cold,  easily  sol.  in  hot  H2O  with 
decomp.  (Ullik.) 

+16H2O.  Insol.  in  cold,  difficultly  sol.  in 
hot  H2O.  (Wempe,  Z.  anorg.  1912,  78.  318.) 

Cerium  molybdate,  Ce2(MoO4)3. 

Precipitate.  Insol.  in  H2O;  sol.  in  acids. 
(Cossa,  B.  19.  536  R.) 

Chromic  molybdate. 

Insol.  in  H2O,  but  sol.  in  acids.  Sol.  in  NH4 
molybdate +Aq.  (Berzelius.) 

See  also  Chromicomolybdic  acid. 

Chromic  molybdate,  with  M.  molybdate. 
See  Chromicomolybdate.    M. 

Cobaltous  molybdate,  CoMoO4. 

Decomp.  by  alkalies  and  strong  acids. 
(Berzelius.) 

+H20.  SI.  sol.  in  pure,  easily  sol.  in  acidi- 
fied H2O.  (Coloriano,  Bull.  Soc.  (2)  50. 
451.) 

CoO,  2MoO3+2H2O.  (Marckwald,  Dis- 
sert. 1895.) 

6^H2O.    SI.  sol.  in  H2O.    (Marckwald.) 

CoMo3O10+10H2O.  Very  si.  sol.  in  cold, 
but  very  easily  sol.  in  hot  H2O.  (Ullik,  W. 
A.  B.  56,  2.  767.) 

Cobaltic  potassium  molybdate. 
See  Cobaltimolybdate,  potassium. 

Cobaltous  sodium  molybdate, 

Na2O,  2CoO,  6MoO3-{-18H2O. 

(Marckwald,  Dissert.  1895.) 

2Na2O,  CoO,  7MoO3+20H2O.  Sol.  in 
cold  H2O  without  decomp.  Decomp.  on 
heating.  (Marckwald.) 


528 


MOLYBDATE  AMMONIA,  COBALTOUS 


3Na2O,  2CoO,  12MoO3+27H2O.  (Marck- 
wald.) 

3Na2O,  3CoO,  14MoO3+50H2O.  Sol.  in 
much  cold  H2O.  (Marckwald.) 

4Na2O,  6CoO,  25MoO3+68H2O.  (Marck- 
wald.) 

Cobaltous    molybdate    ammonia,    CoMoO4, 

2NH3+H2O. 
Sol.   in  H2O.      (Sonnenschein,   J.   pr.   53. 
340.)  - 

Cupric   molybdate,   basic,   4CuO,   3MoO3  + 

5H2O. 
Insol.  in  H2O.    (Struve,  J.  B.  1854.  350.) 

Cupric  molybdate,  CuMoO4. 

81.  sol.  in.H2O;  decomp.  by  acids  and 
alkaline  solutions. 

CuMo3Oi9+6^H2O.  Easily  sol.  in  cold 
H20.  (Ullik,  A.  144.  233.) 

+9H2O.  Very  si.  sol.  in  cold,  and  ex- 
traordinarily easily  sol.  in  hot  H2O.  (Ullik.) 

Cupric  molybdate  ammonia, 
CuMoO4,  2NH3+H2O. 

Gives  off  NH3  at  ord.  temp.  Decomp. 
by  H2O. 

Sol.  in  dil.  NH4OH+Aq  from  which  it  can 
be  cryst.  (Briggs,  Chem.  Soc.  1904,  85.  674.)' 

CuMoO4,  4NH3.  Decomp.  by  H2O.  Sol. 
in  dil.  NH4OH+Aq.  (Jorgensen,  Ch.  Z. 
Repert.  1896,  20.  225.) 

Didymium  molybdate,  Di2(MoO4)8. 

Ppt.    Insol.  in  H2O.    (Cossa,  B.  19.  536R.) 
Di2O3,     6MoO3  +  3H2O  (?).       Precipitate. 

(Smith.) 

Glucinum  molybdate,  basic,  2G1O,  MoO3  + 

3H20. 

Nearly  insol.  in  H2O.  (Atterberg,  J.  B. 
1873.  258.) 

Glucinum  molybdate,  GlO,s  Mo03+2H2O. 

Sol.  in  H2O  with  decomp.  (Rosenheim, 
Z.  anorg.  1897,  15.  307.) 

GlMoO4,  MoO8+^H2O.  Easily  sol.  in 
H2O.  (Atterberg.) 

Gold  (auric)  molybdate  (?). 

81.  sol.  in  H2O.  Sol.  in  HC1,  and  HNO3  + 
Aq.  (Richter.) 

Hydroxylamine  potassium  molybdate. 

Mo04H2(NH30)3(NH2OK). 
Easily  sol.  in  H2O;  pptd.  by  alcohol.    (Hof- 
mann,  A.  1899,  309.  324.) 

Indium  molybdate,   rn2(MoO4)3+2H2O. 
Ppt.    Insol.  in  H2O. 
Easily  sol.  in  HC1.     (Renz,  B.  1901,  34. 

2765.) 


Iron  (ferrous)  molybdate,  FeMoO4. 
Insol.  in  H2O.    (Schultze,  A.  126.  55.) 

Iron    (ferric)    molybdate,    Fe2O3,    4MoO3  + 
7H2O. 

Nearly  insol.  in  H2O.    Slowly  sol.  in  cold, 
easily  in  hot  HC1,  or  HNO3+Aq.    Dil.  acids 
gradually   dissolve  out   Fe2O3  in  the   cold. 
When  ignited,  difficultly  sol.  in  all  solvents. 
(Steinacker.) 

Fe2O3,  5MoO3  +  16H2O.  Very'  si.  sol.  in 
H2O.  (Struve,  J.  B.  1854.  346.) 

2Fe2O3,  7MoO3+34H2O.  Ppt.  (Hall,  J. 
Am.  Chem.  Soc.  1907,  29.  704.) 

Ferric  potassium  molybdate,  Fe2O3,   3K2O, 
12MoO3 +20H2O  =  3K2Mo2O7, 
Fe2(Mo2O7)3+20H2O. 
Sol.  inH2O.    (Struve.) 

Lanthanum    molybdate,    LaH3(MoO4)3  = 

La2O3,  MoO3+3H2O.  (?) 
Precipitate.    (Smith.) 

Lead  molybdate,  PbMoO4. 

Insol.  in  H2O.  Sol.  in  warm  HNO3+Aq; 
decomp.  by  H2SO4;  sol.  in  cone.  HCl+Aq,  or 
KOH+Aq. 

Min.  Wulfenite.    As  above. 

Lithium  molybdate,  Li2MoO4. 

Moderately  sol.  in  cold,  and  only  si.  more 
sol.  in  hot  H2O.  (Ephraim,  Z.  anorg.  1909, 
64.  259.) 

+2/*H2O.    Easily  sol.  in  H2O. 

5Li2O,  5MoO3  +2H2O.  46. 13  g.  are  present 
in  100  ccm.  of  the  aqueous  solution  at  20°, 
and  sp.  gr.  of  the  solution  =  1.44.  (Wempe, 
Z.  anorg.  1912,  78.  309.) 

Li2O,  2MoO3+5H2O.  Sol.  in  cold,  easily 
sol.  in  hot  H2O.  (Ephraim,  Z.  anorg.  1909, 
64.  258.) 

Li2O,  3MoO3+H2O.  Easily  sol.  in  warm 
H2O.  (Wempe,  Dissert.  1911.) 

+4H2O.     (Wempe.) 

+4MH2O.     (Wempe.) 

+7H2O.  Nearly  insol.  in  cold,  sol.  in 
hot  H2O.  (Ephraim,  Z.  anorg.  1909,  64. 
258.) 

2Li2O,  3MoO3.  81.  sol.  in  H2O.  (Ephraim, 
Z.  anorg.  1909,  64.  258.) 

Lithium    paramolybdate,    3Li2O,    7MoO3-f- 

12H2O. 

Sol.  in  H2O.  (Rosenheim,  Z.  anorg.  1897, 
15.  181.) 

+28H2O.  Easily  sol.  in  cold  and  hot  H2O. 
Ephraim,  Z.  anorg.  1909,  64.  258.) 

Lithium  teiramolybdate,  Li2O,  4MoO3+7H2O. 

Sol.  in  cold  H2O.  (Ephraim,  Z.  anorg. 
1909,  64.  258.) 

Li2O,  H2O,  8MoO3+10H2O.     Easily  sol. 


MOLYBDATE,  POTASSIUM 


529 


in  hot  H2O.     (Wempe,  Z.  anorg.  1912,  78. 
308.) 

Li2O,  3H2O,  16MoO3+6^H2O.  Easily 
sol.  in  warm  H2O.  (Wempe,  Z.  anorg.  1912, 
78.  308.) 

Lithium  potassium  molybdate,  KLiMoO4+ 

H2O. 
(Traube,  N.  Jahrb.  Miner,  1894,  I.  194.) 

Magnesium  molybdate,  MgMoO4. 

Min.    Belonesia. 

Insol.  in  HCl+Aq.  (Scacchi,  Zeit.  Kryst. 
1888,  14.  523.) 

+5H2O.  Easily  sol.  in  cold,  but  still  more 
sol.  in  hot  H2O.  (Delafontaine.) 

Sol.  in  12-15  pts.  cold  H2O.    (Brandes.) 

+7H2O.  Easily  sol.  in  hot  or  cold  H2O. 
(Ullik.) 

MgMo3Oi9-j-10H20.  Difficultly  sol.  in 
cold,  very  easily  in  hot  H2O.  (Ullik.) 

Magnesium    paramolybdate,    Mg3Mo7O24+ 

20H2O. 

Quite  sol.  in  cold,  more  easily  in  hot  H2O. 
(Ullik.) 

Magnesium  teframolybdate, 

MgO,  H2O,  8MoO3  +  19H2O. 

Magnesium    hydrogen    fe£ramolybdate, 
MgH2(Mo4O13)2+19H2O. 

Easily  sol.  in  cold  H2O.  (Ullik,  A.  144. 
335.) 

SI.  sol.  in  cold,  easily  sol.  in  hot  H2O. 
(Wempe,  Dissert.  1911.) 

+20H2O.  Ppt.  (Wempe,  Z.  anorg.  1912, 
78.  323.) 

Magnesium  hydrogen  octomolybdate, 

MgH2(Mo8O26)2+29H2O. 
Very  difficultly  sol.  in  cold,  very  easily  sol. 
in  hot  H2O.     (Ullik,  W.  A.  B.  60,  2.  314.) 

Magnesium  potassium  molybdate,  MgMoO4, 

K2MoO4+2H2O. 

Slowly  sol.  in  cold,  easily  in  hot  H2O. 
(Ullik,  A.  144.  343.) 

Manganous  molybdate,  MnMoO4+H2O. 

Insol.  in  H2O.  SI.  sol.  in  pure,  easily  sol. 
in  acidified  H2O.  Decomp.  by  alkalies  or 
alkali  carbonates +Aq.  (Coloriano,  Bull.  Soc. 
(2)  50.  451.) 

+VsH2O.    (Marckwald,  Dissert.  1895.) 

+10H2O.    (Marckwald.) 

Manganic  potassium  molybdate. 
See  Permanganomolybdate,   potassium. 

Manganic  silver  molybdate. 
See  Permanganomolybdate,   silver. 

Mercurous  molybdate,  Hg2Mo2O7. 

Decomp.  by  H2O.  (Struve,  J.  B.  1754. 
350,) 


Sol.   in   500-600  pts.   H2O;   decomp.   by 
HNO3+Aq.     (Hatchett.) 

Molybdenum  molybdate. 

See  Molybdenum  oxides,  Mo3O7,  Mo4Oo, 
etc. 

Neodymium  molybdate,  Nd2(MoO4)3. 
Very  si.  sol.  in  H2O. 

1  pt.  is  sol.  in  53790  pts.  H2O  at  28°. 

1    "  "   "    "  32466    "    H2O    "75°. 
(Hitchcock,  J.  Am.  Chem.  Soc.  1895,  17.  532.) 


Nickel  molybdate,  NiMoO4+2/3H2O,  - 
and  +5H2O. 

(Marckwald,  Dissert.  1895.) 

NiO,  3MoO3+18H2O.  SI.  sol.  in  cold;  easily 
sol.  in  hot  H2O.  (Marckwald.) 

5NiO,  14MoO3+57H2O.  and  +70H2O. 
SI.  sol.  in  cold;  easily  sol.  in  not  H2O.  (Marck^ 
wald.) 

Nickel  potasshun  molybdate,  3NiO,   5K2O 

16MoO3+21H2O. 

Can  be  cryst.  from  H2O.  (Hall,  J.  Am. 
Chem.  Soc.  1907,  29.  701.) 

Nickelic  potassium  molybdate. 
See  Nickelimolybdate,  potassium. 

Nickel  potassium  hydrogen  molybdate, 

K4H6[Ni(MoO4)6]  +5H2O. 
See  Nickelomolybdate,   potassium  hydro- 
gen. 

Nickel    sodium    molybdate,    2NiO,     Na2O, 

6MoO3+17H2O. 

Sol.  in  cold  H2O  without  decomp.  but  de- 
comp. on  warming.  (Marckwald,  Dissert. 
1895.) 

Nickel  molybdate  ammonia,  NiMoO4,  2NH3 

+H20. 

Decomp.  by  H2O.  (Sonnenschein,  J.  pr. 
53.  341.) 

Potassium  molybdate,  K2MoO4. 

Deliquescent  in  moist  air.  Very  sol.  in 
H2O.  Insol.  in  alcohol.  (Svanberg  and 
Struve,  J.  pr.  44.  265.) 

184.6  grams  are  sol.  in  100  grams  H2O  at 
25°.  (Amadori,  C.  A.  1912.  2878.) 

Solubility  of  K2MoO4+K2SO4  at  25°. 


G.  per  100  g.  H2O 

G.  per  100  g.  H2O 

K2S04 

K2MoO4 

K2S04 

K2MoO< 

0 
0.46    - 
0.72 
0.98 
1.27 

184.6 
180.7 
177. 
127.2 
107.5 

1.50 
2.13 
3.95 

8.55 
12.10 

99.49 
45.89 
17.48 
4.73 
0 

(Amadori,  Att.  ace.  Line.  1912,  21,  I.  467, 
667.) 


530 


MOLYBDATE,  POTASSIUM 


Easily  sol.  in  H2O.  (Wempe, 
Dissert.  1911.) 

K2O,  8MoO3+13H2O.  Easily  sol.  in 
warm  H2O.  (Wempe,  Dissert.  1911.) 

K2O,  10MoO3+9H2O.  Nearly  insol.  in 
hot  and  cold  H2O.  100  g.  H2O  dissolve 
0.682  g.  at  100°.  (Felix,  Dissert,  1912.) 

+15H2O.    Sol.  inH2O.    (Felix.) 

5K2O,  12MoO3+8H2O.  SI.  sol.  in  cold 
H2O.  (Junius,  Z.  anorg.  1905,  46.  439.) 

Potassium  inmolybdate,  K2Mo3Oio. 

Difficultly  sol.  in  cold,  but  much  more  easily 
in  hot  H2O.  When  ignited  is  absolutely  insol. 
in  H2O.  (Svanberg  and  Struve.) 

+2H2O.    (Junius,  Z.  anorg.  1905,  46.  439.) 

SI.  sol.  in  cold,  easily  sol.  in  hot  H2O. 
(Wempe,  Dissert.  1911.) " 

+2MH2O.  Easily  sol.  in  H2O.  (Wempe, 
Dissert.  1911.) 

+3H2O.  Very  si.  sol.  in  cold,  more  easily 
sol.  in  hot  H2O.  (Wempe,  Dissert.  1911.) 

+11H2O.  Practically  insol.  in  H2O. 
(Westphal,  Dissert.  1895.) 

Potassium  hydrogen  teframolybdate. 

K6H4[H2(Mo2O7)6]+18H2O. 

SI.  sol.  in  cold  H2O.  Decomp.  by  boiling 
H2O.  (Rosenheim,  Z.  anorg.  1913,  79.  298.) 

KHMo4O13+6H2O.  Decomp.  by  H2O. 
(Ullik'.) 

Potassium  paramolybdate,  K6Mo7O24  + 
4H2O. 

Decomp.  even  by  cold  H2O.  (Delafon- 
taine.) 

Formula  is  KgMogOsi  +6H2O,  according  to 
Svanberg  and  Struve  (?). 

Potassium  selenium  molybdate. 
See  Selenomolybdate,  potassium. 

Potassium     sodium     molybdate,     K2MoO4, 

2Na2MoO4+14H2O. 

Very  easily  sol.  in  cold,  still  more  easily  in 
hot  H2O.  (Delafontaine.) 

Potassium  vanadium  molybdate. 
See  Vanadiomolybdate,  potassium. 

Potassium  zinc  molybdate. 
Sol.  in  H2O.    (Berzelius.) 

Potassium     molybdate     hydrogen     rftoxide, 

6K2O,  16MoO3,  4H2O2  +  13H2O. 
Sol.  in  H2O.    (Barwald,  C.  C.  1885.  424.) 

Potassium  molybdate  sulphocyanide.  KSCN, 

K2Mo3O10+4H2O. 

Decomp.  by  H2O.  Sol.  in  dil.  HCl+Aq. 
(Pechard,  C.  R.  1894,  118.  806.) 


Praseodymium  molybdate,  Pr2(MoO4)3. 
Very  si.  sol.  in  H2O. 
1  pt.  is  sol.  in  65820  pts.  H2O  at  23°. 
1  "    "    "    "  69800    "       "      "  75°. 

(Hitchcock,  J.  Am.  Chem.  Soc.  1895,  17. 
530.) 

Rubidium  molybdate,  Rb2O,  MoO3. 

Hygroscopic.  (Ephraim,  Z.  anorg.  1909, 
64.  263.) 

Rb2O,  2MoO3+2H2O.  Easily  sol.  in  H2O. 
(Ephraim,  Z.  anorg.  1909,  64.  263.) 

Rb6Mo7O24+4H2O.  Very  si.  sol.  in  cold, 
much  more  easily  sol.  in  hot  H2O.  (Dela- 
fontaine, N.  Arch.  Sc.  phys.  nat.  30.  233.) 

(Ephraim,  Z.  anorg.  1909,  64.  263.) 

+42/3H2O.    (Wempe,  Dissert.  1911.) 

2Rb2O,  7MoO3+5H2O.  Very  si.  sol.  in 
cold,  very  easily  sol.  in  hot  H2O.  (Wempe.) 

5Rb2O,  7MoO3+14H2O.  (Ephraim  and 
Herschfinkel,  Z.  anorg.  1909,  64.  268.) 

3Rb2O,  8Mo03+6H2O.  (Ephraim  and 
Herschfinkel,  Z.  anorg.  1909,  64.  269.) 

5Rb2O,  12MoO3+H2O.  100  cc.  H2O  dis- 
solve 1.941  g.  at  24°.  (Wempe,  Z.  anorg. 
1912,  78.  258.) 

Rb2O,  3MoO3.  Insol.  in  H2O.  (Muth- 
mann,  B.  1898,  31.  1839.) 

+H20.    (Muthmann,  B.  1898,  31.  1839.) 

-j-3H2O.  SI.  sol.  in  cold,  easily  sol.  in  hot 
H2O.  (Wempe,  Dissert.  1911.) 

6^H2O.  (Ephraim  and  Herschfinkel,  Z. 
anorg.  1909,  64.  269.) 

2Rb2O,  3MoO3+4H2O.  SI.  sol.  in  cold, 
easily  in  hot  H2O.  (Wempe,  Dissert.  1911.) 

Rb2O,  4MoO3.  Difficultly  sol.  in  cold, 
easily  in  hot  H2O.  (Wempe,  Z.  anorg.  1912, 
78.  312.) 

+  ^H2O.  Practically  insol.  in  H20.  Very 
sol.  by  addition  of  NH3.  (Ephraim  and 
Herschfinkel,  Z.  anorg.  1909,  64.  266.) 

+2.5H2O.  Insol.  in  H2O.  (Ephraim,  Z. 
anorg.  1909,  64.  263.) 

+4H2O.  Sol.  in  cold,  more  easily  sol.  in 
hot  H2O.  (Wempe,  Z.  anorg.  1912,  78.  312.) 

Rb2O,  MoO3,  Rb2O,  3MoO3+5H2O.  Sol. 
in  cold  or  hot  H2O.  (Wempe,  Z.  anorg.  1912, 
78.  312.) 

Rb2O,  H2O,  8MoO3+3H2O.  Difficultly 
sol.  in  cold,  easily  in  hot  H2O.  (Wempe,  Z. 
anorg.  1912,  78.  312.) 

Rb2O,  HMoO3+5.5H2O.  Ppt.  (Ephraim, 
Z.  anorg.  1909,  64.  263.) 

Rb2O,  13MoO3+4H2O.    Ppt.    (Ephraim.) 

Rb2O,  18MoO3.    Ppt.    (Ephraim.) 

Samarium  molybdate,  Sm2(MoO4)3. 
Insol.  in  H2O.    (Cleve.) 

Samarium  sodium  molybdate, 

Na2Sm2(MoO4)4. 

Insol.  in  H2O.  Easily  sol.  in  warm  dil. 
HN03+Aq.  (Cleve.) 


MOLYBDATE  MOLYBDENUM  OXIDE  SODIUM 


531 


Silver  (argentous)  molybdate,  Ag4O,  2MoO3. 

Sol.  in  HNO3+Aq.  KOH+Aq  dissolves 
MoO3  and  Ag4O  separates  out.  Not  decomp. 
by  dil.  NH4OH+Aq.  (Wohler  and  Rauten- 
berg,  A.  114.  119.) 

Does  not  exist.    (Muthmann,  B.  20.  983.) 

Silver  (argentic)  molybdate,  Ag2MoO4. 

Somewhat  sol.  in  H2O;  less  when  HNO3  is 
present.  (Richter.) 

Very  si.  sol.  in  pure  H2O;  easily  sol.  in 
H2O  acidulated  with  HNO3.  (Struve  and 
Svanberg.) 

Sol.  in  KCN  or  NaOH+Aq.  (Smith  and 
Bradbury.) 

Ag2O,  2MoO3.  SI.  sol.  in  H2O.  Sol.  in 
KCN+Aq.  (Junius,  Dissert.  1905.) 

2Ag2O,  5MoO3.  Somewhat  sol.  in  H2O. 
(Svanberg  and  Struve,  J.  B.  1847-48.  412.) 

Ag2O,  4MoO3-f  6H2O.  SI.  sol.  in  H2O  with 
decomp.  (Wempe,  Z.  anorg.  1912,  78.  322.) 

Silver  thorium  molybdate. 
See  Thoromolybdate,  silver. 

Silver  molybdate  ammonia,  Ag2MoO4,  4NH3. 
Sol.    in    H2O    with   rapid    decomposition. 
(Widmann,  Bull.  Soc.  (2)  20.  64.) 

Silver  molybdate  hydrogen  dioxide,  13Ag2O, 

2H2O2,  32MoO3. 
Ppt.    (Barwald,  B.  1,7.  1206.) 

Sodium  molybdate,  Na2MoO4. 

Anhydrous.  Easily  and  completely  sol.  in 
H2O. 

+2H2O.    Sol.  inH2O. 

+10H2O.    Efflorescent. 

Solubility  in  H2O  at  t°. 


oe 
^  3 

3  • 

•g! 

sl 

0^2 
•S  § 

+a   03 

gifi 

Solid  phase 

t    . 

i| 

w§| 

l8S 

fej>> 

^06   O 

"°2 

rt 

*f* 

|s 

Na2MoO4,  102HO 

0 

30.63 

25.92 

3.86 

u 

4 

33.83 

22.38 

4.47 

11 

6 

35.58 

20.72 

4.83 

u 

90 

38.16 

18.54 

5.39 

Na2MoO4,  2H2O 

10 

39.28 

17.70 

5.65 

" 

15.5 

39.27 

17.70 

5.65 

M 

32. 

39.82 

17.30 

5.78 

" 

51.5 

41.27 

16.28 

6.14 

" 

100 

45.57 

13.67 

7.32 

(Funk,  B.  1900,  33.  3699.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Na2Mo2O7.  After  ignition,  very  difficultly 
sol.  in  cold,  and  very  slowly  sol.  in  hot  H2O. 
(Svanberg  and  Struve.) 

+H2O.    Easily  sol.  in  H2O. 


Easily  sol.  in  cold  or  hot  H2O. 
(Wempe,  Dissert.  1911.) 

-|-4H2O.  Easily  and  completelv  sol.  in 
coldH2O.  (Ullik.) 

+6^H2O.  SI.  sol.  in  cold,  very  easily  sol. 
in  hot  H2O.  (Wempe,  Dissert.  1911.) 

+7H2O.  Difficultly  sol.  in  cold  H2O,  but 
more  easily  than  the  corresponding  K  salt. 
100  pts.  H2O  dissolve  3.878  pts.  at  20°  and 
13.7  pts.  at  100°.  (Ullik,  A.  144.  244.) 

+9H2O.  Easily  sol.  in  cold,  very  easily 
sol.  in  hot  H20.  (Wempe.) 

+11H2O.  (Junius,  Z.  anorg.  1905,  46. 
437.) 

3Na20,  7MoO3.  Easily  sol.  in  cold,  very 
easily  sol.  in  hot  H2O.  (Ott,  Dissert.  1911.) 

+20H2O.    (Westphal,*  Dissert.  1895.) 

+22H2O.  Efflorescent.  Easily  sol.  in 
H2O.  (Ullik,  A.«144.  219.) 

Na2O,  8MoO3  +  3^H2O.  Very  sol.  in  cold 
or  hot  H20.  (Wempe,  Dissert.  1911.) 

+4H20.  Insol. 'in  H2O.  (Ullik,  W.  A.  B. 
60,  2.  312.) 

+15H2O.  (Rosenheim,  Z.  anorg.  1897,  15. 
188.) 

Na2O,  10MoO3+6H2O.  Very  si.  sol.  in 
H2O.  100  g.  H2O  dissolve  0.842  g.  at  100°. 
(Felix,  Dissert.  1912.) 

+7H2O.  (Felix.)  Nearly  insol.  in  hot  and 
cold  H2O.  (Rosenheim,  Z.  anorg.  1903,  37. 
323.) 

+12H2O.    Difficultly  sol.  in  H2O. 

-f  21H2O.  Abundantly  but  slowly  sol.  in 
coldH20.  =  NaHNa5016+10H20.  (Ullik.) 

5Na2O,  12MoO3+8H2O.  SI.  sol.  in  cold, 
easily  sol.  in  hot  H2O.  (Wempe,  Dissert. 
1911.) 

+20H2O.  SI.  sol.  in  cold,  easily  sol.  in 
hot  H2O.  (Wempe,  Dissert.  1911.) 

+36H2O.    (Junius,  Z.  anorg.  1905,  46.  436.) 

+44H2O.  SI.  sol.  in  cold,  easily  sol.  in  hot 
H2O.  (Wempe,  Dissert.  1911.) 

Sodium  teframolybdate,  Na2Mo4Oi3+6H2O. 

Difficultly  sol.  in  cold,  easily  in  hot  H2O. 
(Ullik.) 

100  cc.  H2O  dissolve  at  21°,  28.39  g. 
of  the  salt.  Sp.  gr.  of  the  solution  =  1.47. 
(Wempe,  Z.  anorg.  1912,  78.  306.) 

-f  17H2O.    (Felix,  Dissert.  1912.) 

Na6H4[H2(Mo2O7)6]+21H2O.  Slowly  sol. 
in  cold,  easily  sol.  in  hot  H2O.  (Rosenheim, 
Z.  anorg.  1913,  79.  298.) 

NaHMo4Oi3+8H2O.  Very  sol.  in  hot  or 
cold  H2O.  (Ullik,  A.  144.  333.) 

NaHMo8O26  +  4H2O.  Insol.  in  H2O. 
(Ullik.) 

Sodium  manganous  molybdate,  2Na2O,  MnO, 

6MoO3-H9H2O. 
(Marckwald,  Dissert.  1895.) 

Sodium   molybdate   molybdenum   oxide, 

Na2Mo5Oi5. 

Insol.  in  H2O.  Sol.  in  HNO3  and  aqua 
regia.  Insol.  in  HC1  and  in  H2SO4.  Sol.  in 


532 


MOLYBDATE,  STRONTIUM 


alkalies.    (Stavenhagen  and  Engels,  B.  1895, 
28.  2280.) 

Strontium  molybdate,  SrMoO4. 

SI.  sol.  in  H2O.    (Schultze.) 

Sol.  in  9600  pts.  H2O  at  17°.  (Smith  and 
Bradbury,  B.  24.  2930.) 

SrO,  3MoO3  +  KH2O.  Scarcely  sol.  in  cold, 
easily  in  hot  H2O.  (Wempe,  Dissert.  1911.) 

SrO,  H2O,  8MoO3+6H2O.  Scarcely  sol. 
in  cold,  easily  in  hot  H2O.  (Wempe,  Dissert. 
1911.) 

2SrO,  3H2O,  20MoO3+21H2O.     Ppt. 
(Wempe,  Z.  anorg.  1912,  78.  321.) 

Thallous  molybdate,  Tl2MoO4. 

Insol.  in  H2O.  Sol.  in  alkalies.  Insol.  in 
alcohol.  (Oettinger,  J.  B.  1864,  254.) 

SI.  sol.  in  hot  or  cold  H2O.  (Ullik,  J.  B. 
1867,  234.) 

8T12O,  llMoO3.  Sol.  in  hot  H2O.  (Flem- 
ing, J.  B.  1868,  250.) 

3T12O,  8MoO3.    (Fleming.) 

Thallous  teframolybdate,  T12O,  4MoO3+H2O. 
SI.  sol.  in  H2O  with  decomp.     (Wempe, 
Z.  anorg.  1912,  78.  322.) 

Thallous  paramolybdate,  5T12O,  12MoO3. 

Insol.  in  H2O.  Easily  sol.  in  mineral  acids 
and  in  alkali  hydroxides  and  carbonates. 
(Junius,  Z.  anorg.  1905,  46.  432.) 

Tin  (stannic)  molybdate. 

Insol.  in  H2O.  Sol.  in  dil.  or  cone.  HC1+ 
Aq,  or  in  KOH+Aq.  Not  decomp.  by  HNO3 
+Aq.  (Berzelius.) 

Uranous  molybdate. 

Precipitate.  Sol.  in  HCl+Aq.  Decomp. 
by  KOH+Aq. 

U(MoO4)2.    (Lancien,  C.  C.  1908,  I.  1763.) 

Uranyl  molybdate,  (UO2)MoO4. 

Insol.  in  H2O,  methyl  and  ethyl  alcohol, 
ether,  acetic  acid?  CHC13,  CeHe  and  CyHs. 
Sol.  in  mineral  acids.  (Lancien,  C.  C.  1907. 
I.  784.) 

2UO3,  3MoO3  (?).  Insol.  in  H2O.  Sol.  in 
strong  acids  and  (NH4)2CO3+Aq.  (Ber- 
zelius.) 

3UO3,  7MoO3.  Insol.  in  hot  and  cold  H2O. 
Insol.  in  NaOH,  KOH,  and  NH4OH+Aq. 
Sol.  in  all  min.  acids  and  decomp.  by  an  ex- 
cess of  H2O.  Insol.  in  acetic  acid.  (Lancien, 
C.  C.  1908, 1.  1763.) 

UO3,  8MoO3.    (Lancien.) 

+13H2O.     Insol.  in  HNO3.     (Lancien.) 

Ytterbium  molybdate,  Yb2O3,  7MoO3+6H2O. 

Insol.  in  hot  H2O.  (Cleve,  Z.  anorg.  1902, 
32.  152.) 

2Yb2O3,  MoO3.    Ppt.    (Cleve.) 


Yttrium  molybdate. 

Insol.  in  H2O.  Sol.  in  HNO3+Aq.  (Ber- 
lin.) 

Zinc  molybdate,  ZnMoO4. 

Difficultly  sol.  in  H2O;  easily  in  acids. 
(Schultze,  A.  126.  49.) 

+H2O.  SI.  sol.  in  H2O.  Easily  sol.  in 
dil.  acids.  (Coloriano,  Bull.  Soc.  (2)  50.  451.) 

ZnMo3O19+10H2O.  yery  difficultly  sol. 
in  cold,  but  extraordinarily  easily  sol.  in  hot 
H2O.  (Ullik,  W.  A.  B.  55,  2.  767.) 

Zinc  teframolybdate,  ZnMo4O13+8H2O. 
Easily  sol.  in  cold  H2O.    (Ullik.) 
ZnO,H2O,8MoO3+14H2O.    Ppt.  (Wempe, 

Z.  anorg.  1912,  78.  324.) 

Zinc  molybdate  ammonia,  ZnMoO4,  2NH3  + 

H2O. 
(Sonnenschein,  J.  pr.  53.  339.) 

Pmnolybdic  acid. 
See  Permolybdic  acid. 

Molybdic  sulphuric  acid,  MoO3,  S03. 
Deliquescent.     (Schultz-Sellack,  B.  4.  14.) 
Very    deliquescent.      Very    sol.    in    H20. 

(Muthmann,  A.  1886,  238.  126.) 
MoO3,  3SO3+2H2O  (?). 

Molybdocyanhydric  acid,  H4Mo(CN)8-f 

6H2O. 

Easily  sol.  in  H2O  and  abs.  alcohol.  Solu- 
tions are  stable  at  ord.  temp.  (Rosenheim 
and  Garfunkel,  Z.  anorg.  1910,  65.  168.) 

Cadmium   molybdocyanide,    Cd2Mo(CN)8+ 

8H2O. 
Insol.  in  H2O.    (Rosenheim.) 

Cadmium  molybdocyanide  ammonia, 

Cd2Mo(CN)8,  4NH3+2H2O. 
(Rosenheim.) 

Cupric  molybdocyanide  ammonia, 

Cu2Mo(CN)8,  4NH3+7H2O. 
(Rosenheim.) 

Potassium   molybdocyanide,    K4Mo(CN)8+ 

2H20. 
Very  sol.  in  H2O.    (Rosenheim.) 

Thallous  molybdocyanide,  Tl4Mo(CN)8. 
Very  si.  sol.  in  H2O.    (Rosenheim.) 

Molybdoiodic  acid,  HIO3,  H2MoO4+H2O. 

Easily  sol.  in  H2O.  (Blomstrand,  J.  pr.  (2) 
40.  320.) 

I2O5,  2MoO3+2H2O.  Very  sol.  in  H2O. 
Insol.  in  cold,  sol.  in  hot  HNO3.  Sol.  in  al- 
cohol. (Chretien,  A.  ch.  1898,  (7)  15..  402.) 


MOLYBDOIODATE,  ZINC 


533 


Ammonium  molybdoiodate,  NH4IO3, 
H2MoO4. 

Somewhat  more  sol.  than  K  salt.  (Blom- 
strand.) 

(NH4)2O,  I2O5,  2MoO3.  Very  si.  sol.  in 
cold  H2O.  More  sol.  in  hot  H2O.  (Rosen- 
heim  and  Liebknechfc,  A.  1899,  308.  50.) 

+H2O.  1  1.  H2O  dissolves  5.39  g.  salt  at 
15°;  30.94  g.  at  100°.  More  sol.  in  dil.  HNO3 
+Aq.  (Chretien,  A.  ch.  1898,  (7)  15.  409.) 

3(NH4)20,  (1,0,,  2Mo03)4+6H20.  (Chr6- 
tien.) 

Barium  molybdoiodate,  BaO,  12O5,  2MoO3-f 

2H2O. 
4.23  g.  are  sol.  in  1  1.  H2O  at  ord.  temp. 

(Chretien.) 

Cadmium  molybdoiodate,  acid,  3CdO,  (I2O5, 

2MoO3)6+16H20. 
SI.  sol.  in  H2O.    (Chretien.) 

Calcium  molybdoiodate,  CaO,  I2O5,  2MoO3  + 

6H2O. 

1  1.  H2O  dissolves  7.8  g.  of  the  salt  at 
15°;  20.89  g.  at  90°.  (Chretien.) 

Cobaltous  molybdoiodate,  CoO,  I2O5,  2Mo03 

+6H2O. 

5.11  g.  are  sol.  in  1  1.  H2O  at  15°;  22.27  g. 
at  100°.  (Chretien.) 

Cobaltous  molybdoiodate  acid,  CoO,   (I2O5, 

2MoO3)5+18H2O. 
Very  sol.  in  H2O.    (Chretien.) 

Cupric  molybdoiodate,  CuO,  I2O5,  2MoO3  + 

3H2O. 

1  1.  H2O  dissolves  10.63  g.  of  the  salt  at 
15°;  25.55  g.  at  100°.  (Chretien.) 

Lithium  molybdoiodate,  Li2O,  I2O5,  2MoO3  + 


197.83  g.  are  sol.  in  1  1.  H2O  at  15°.  Sol.  in 
dil.  HNO3+Ag.  (Chretien.) 

Magnesium  molybdoiodate,  MgO,   I2O6, 

2MoO3+6H2O. 

1  1.  H2O  dissolves  3.85  g.  of  the  salt  at 
15°;  18.2  g.  at  100°.  (Chretien.) 

Manganous    molybdoiodate,    3MnO,    (I205, 

2MoO3)4+9H2O. 

1  1.  H2O  dissolves  17.05  g.  of  the  salt  at 
15°;  55.05  g.  at  100°.  (Chretien.) 

Nickel  molybdoiodate,  NiO,  I2O5,  2MoO3 
6H2O. 

5.43  g.  are  sol.  in  1  1.  H2O  at  15°;  21.8  g.  at 
100°.  (Chretien.) 

2NiO,  2IjO6,  3MoO3+23H2O.  Easily  sol. 
in  H2O.  Not  decomp.  by  acids.  (Maass, 
Dissert.  1901.) 


Nickel    molybdoiodate,    acid,    2NiO,    (I2O5, 

2MoO3)5+15H2O. 
Very  sol.  in  H2O.    (Chretien.) 

Potassium  molybdoiodate, 

KHO2IO2MoO3OH,    or   KIO3,    MoO3-f- 
2H20. 

Ppt.  SI.  sol.  in  H2O.  (Blomstrand,  J.  pr. 
2)  40.  320.) 

K2O,  I2O5,  2Mo03.  Only  si.  sol.  in  cold 
H2O;  sol.  on  long  boiling.  4.48  grs.  are  sol. 
in  1  1.  H2O  at  12°.  (Compare  Blomstrand: 
not  identical.)  (Rosenheim,  A.  1899,  308. 
50.) 

+H2O.  SI.  sol.  in  H2O.  3.45  g.  are  sol. 
in  1  1.  H2O  at  15°;  28.38  g.  at  100°.  More 
sol.  in  dil.  HNO3+Aq.  (Chretien,  A.  ch. 
1898,  (7)  16.  404.) 

Potassium  molybdoiodate,  acid. 
(I2O5,  2Mo03)6,  4K2O+7H2O. 
(I2O5,  2MoO3)3,  2K2O  +  13H2O. 
(I2O5,  2MoO3)2,  K2O+4H2O. 
(I2O5,  2MoO3)3,  K2O+7H2O. 
(I2O6,  2MoO3)4,  K2O+5H2O. 
(Chretien.) 

Silver  molybdoiodate,  Ag2O,  I2O5,  2MoO3-h 


Insol.  in  H2O. 

4Ag2O,  4I2O5,  3MoO3.  Sol.  in  H2O  con- 
taming  HNO3.  (Chretien.) 

Sodium  molybdoiodate,  Na2O,  I2O5,  2MoO3+ 
H2O. 

SI.  sol.  in  H2O.  Sol.  in  HNO3  with  decomp. 
(Chretien,  C.  R.  1896,  123.  178.) 

1  1.  H2O  dissolves  6.97  g.  of  the  salt  at  15°; 
22.75  g.  at  90°. 

1  1.  HNO3+Aq  (1  :  10)  dissolves  23.78  g. 
of  the  salt  at  ord.  temp.  (Chretien,  A.  ch. 
1898,  (7)  15.  410.) 

+2H2O.  Only  si.  sol.  in  cold  H2O;  sol.  on 
long  boiling.  3.35  grams  are  sol.  in  1  1.  H2O 
at  12°.  (Rosenheim,  A.  1899,  308.  50.) 

Strontium  molybdoiodate,  SrO,  I2O6,  2MoO  + 

3H2O. 

Very  sol.  in  H2O.  (Chretien,  A.  ch.  1898, 
(7)  15.  415.) 

Strontium  molybdoiodate,  acid,  3SrO,  (I2O6, 

2MoO3)4+15H2O. 

1  1.  H2O  dissolves  2.94  g.  of  the  salt  at 
15°;  13.64  g.  at  100°.  (Chretien.) 

Uranyl  molybdoiodate,  2UO3,  4I2O6,  3MoO3  + 
3H2O.  (Chretien.) 

Zinc   molybdoiodate,   ZnO,    I2O6,   2MoO3  + 

5H2O. 

1  1.  H2O  dissolves  4.08  g.  of  the  salt  at 
15°;  16.25  g.  at  100°.  (Chretien.) 


534 


MOLYBDOIODATE  ACID,  ZINC 


Zincmolybdoiodate  acid,  ZnO,  (I2O5, 2MoO3)3 

+16H2O. 
Very  sol.  in  H2O.    (Chretien.)     . 

Molybdoperiodic  acid. 

Ammonium  molybdoperiodate,  5(NH4)2O, 
I2O7,  12MoO3+12H2O. 

Sol.  in  H2O.  (Blomstrand,  Sv.  V.  A.  H. 
Bih.  1892.  No.  6.) 

4(NH4)2O,  I2O7,  8MoO3+7H2O.  Very  si. 
sol.  in  cold  H2O.  (Blomstrand.) 

Ammonium  sodium  ,  2(NH4)2O,  Na2O, 

I2O7,  2MoO3+10H2O. 
Very  si.  sol.  in  H2O.    (B.) 

-,  9BaO,   Na2O,  2I2O7, 


Barium  sodium 

24MoO3+28H2O.' 
Very  si.  sol.  in  H2O.    (B.) 

Calcium ,  5CaO,  I2O7,  12MoO3+26H2O. 

Extremely  sol.  in  H2O.    (Blomstrand.) 
4CaO,  I2O7,  12MoO3+21H2O.    Less  sol.  in 

H2O  than  above  salt. 

Lithium ,  5Li2O,  I2O7,  12MoO3+30H2O. 

Not  so  efflorescent  as  Na  salt.    Sol.  in  H2O. 

(B.) 

+  18H20.)    (B.) 


-,    2MnO,    3Na20, 


Manganous    sodium 

I2O7,  12MoO3+32H2O. 
Sol.inH20.    (B.) 

Potassium    ,    5K2O,    I2O7,    12MoO3+ 

12H2O. 
Not  efflorescent.    (Blomstrand.) 

Sodium ,  5Na2O,  I2O7,  12MoO3+34H2O. 

Efflorescent.  Very  sol.  in  H2O.  (Blom- 
strand, Sv.  V.  A.  H.  Bih.  1892.  No.  6.  24.) 

+26H2O.  Not  efflorescent.  Very  sol.  in 
H2O.  (Blomstrand.) 

Sodium  strontium  ,  Na2O,  4SrO,  I2O7, 

12MoO3+20H2O. 
Sol.  inH2O.    (B.) 

Molybdophosphoric  acid. 
See  Phosphomolybdic  acid. 

Molybdosw&phosphoric  acid. 

Sodium  molybdosu&phosphate, 

Na2[P(Mo2O7)3]+8H2O. 
•     Ppt.    (Rosenheim,  Z.  anorg.  1913,  84.  222.) 

Molybdophosphorous  acid. 

Potassium  molybdophosphite, 

K2[HP(Mo2O7)  3]  + 1 1H2O. 
Difficultly  sol.  in  cold  H20.     (Rosenheim, 
Z.  anorg.  1913,  84.  219.) 


Sodium  molybdophosphite, 

Na2[HP(Mo2O7)3]  +  llH2O. 
SI.  sol.  in  H2O.     (Rosenheim,   Z.  anorg. 
1913,  84.  218.) 

Molybdophosphovanadic  acid. 
See  Phosphovanadiomolybdic  acid. 

Molybdoselenious  acid. 

Ammonium    molybdoselenite,    4(NH4)2O, 

3SeO2,  10MoO3+4H2O. 
More  sol.  in  hot  than  cold  H2O;  insol.  in 
alcohol.    (Pechard,  A.  ch.  (6)  30.  403.) 

Ammonium  potassium  molybdoselenite, 

2(NH4)2O,     2K2O,     3SeO2,     10MoO3  + 
5H2O. 

Very  sol.  in  H2O;  insol.  in  alcohol.  (Pech- 
ard.) 

Barium   molybdoselenite,   4BaO,    3SeO2, 

10MoO3+3H2O. 

SI.  sol.  in  cold,  easily  in  warm  H2O. 
(Pechard.) 

Potassium   molybdoselenite,    4K2O,    3SeO2, 

10MoO3+5H2O. 

Very  sol.  in  H2O;  insol.  in  alcohol.  (Pech- 
ard.) 

Sodium    molybdoselenite,     4Na2O,     3SeO2, 

10Mo03  +  15H2O. 

Very  efflorescent,  and  sol.  in  H20;  insol.  in 
alcohol.  (Pechard.) 

Molybdosilicic  acid. 
See  Silicomolybdic  acid. 

Molybdosilicovanadic  acid. 
See  Silicovanadiomolybdic  acid. 

Molybdosulphuric  acid. 

Appreciably  sol.  in  H2O.  (Hoffmann, 
Dissert.  1903.) 

Ammonium  molybdosulphate,   (NH4)2O, 
2MoO3,  SO3+4H2O,  and  +9H2O. 

Decomp.  by  H2O.  (Weinland,  Z.  anorg. 
1907,  64.  261.) 

(NH4)2O,  2MoO3,  3SO3  +  10H2O.  (Wein- 
land.) 

Ammonium  molybdenyl  molybdosulphate, 
(NH4)2O,  MoO2,  7MoO3,  SO3+zH2O. 

1^(NH4)2O,  MoO2,  7MoO3,  SO3+5H2O. 

2(NH4)2O,  MoO2,  7MoO3,  SO3+14H2O. 
(Hoffmann,  Dissert.  1903.) 

3NH3,  MoO2,  7MoO3,  S93+10H2O.  Very 
sol.  in  H2O.  Very  si.  sol.  in  NH4  salts +Aq. 
Very  stable  toward  alkali +Aq.  (Pechard, 
C.  R.  1893,  116.  1441.) 


NEODYMIUM  HYDROXIDE 


535 


5NH3,  MoO2,  7MoO3,  SO3+8H2O.  (Pe- 
chard,  C.  R.  1893,  116.  1441.) 

Potassium  molybdosulphate,  K2O,  2MoO3, 
SO3+2H2O. 

K2O,  2MoO3,  SO3+6H2O. 

K2O,  2MoO3,  3SO3+6H2O.  (Weinland,  Z. 
anorg.  1907,  54.  260.) 

Potassium   molybdenyl   molybdosulphate, 

K2O,  MoO2,  7MoO3,  SO3+8H2O. 
(Hoffmann,  Dissert.  1903.) 

Molyb  do  sulphurous  acid. 

Ammonium    molybdosulphite,    4(NH4)2O, 
3SO2,  10MoO3+6H2O. 

SI.  sol.  in  cold,  more  easily  in  hot  H2O. 
Insol.  in  alcohol.  (Pechard,  "A.  ch.  (6)  30. 
396.) 

3(NH4)2O,  8MoO3,  2SO2+5H2O.  SI.  sol. 
in  cold,  easily  sol.  in  warm  H2O.  Easily  de- 
comp.  by  H2O,  and  can  be  recryst.  only  in 
presence  of  an  excess  of  sulphurous  acid. 
(Rosenheim,  Z..  anorg.  1894,  7.  177.) 

Ammonium  potassium  molybdosulphite, 

2(NH4)2O,  2K2O,  3SO2,  10MoO3+9H2O. 
SI.  sol.  in  cold  H2O.    Decomp.  on  warming. 
(Pechard.) 

Barium     molybdosulphite,     2BaO,     5MoO3, 

2SO2-flOH2O. 
(Rosenheim,  Z.  anorg.  1897,  15.  185.) 

Caesium    molybdosulphite,    2Cs?O,    5MoO3, 

2SO2+6H2O. 
Unstable.    As  K  salt.    (Rosenheim.) 

Potassium  molybdosulphite,  4K2O,  3SO2, 
10Mo03+10H2O. 

Very  si.  sol.  in  H2O,  but  decomp.  on  warm- 
ing. (Pechard.) 

2K2O,  5MoO3,  2SO2+H2O.     (Rosenheim.) 

Rubidium  molybdosulphite,  2Rb2O,  5MoO3, 

2S02  +  ^H20. 
As  K  salt.    (Rosenheim.) 

Sodium  molybdosulphite,  4Na2O,   3SO2, 

10MoO3  +  12H2O. 
Very  sol.  in  cold  H2O;  insol.  in  alcohol. 

(Pechard.) 

+  16H2O.    Very  efflorescent.    (Pechard.) 
2Na2O,  5MpO3,  2SO2+8H2O.    In  dry  state 

it  gradually  gives  off  SO2  and  soon  effloresces. 

(Rosenheim.) 

Strontium   molybdosulphite,   2SrO,    5MoO3, 
H2O. 


+  12 
(Rosenheim.) 

Molybdotitanic  acid. 
See  Titanomolybdic  acid. 


Molyb dous  acid. 

Magnesium   molybdite,  Mg2Mo3O8=2MgO, 

3MoO2. 

Not  attacked  by  KOH,  and  HCl+Aq. 
(Muthmann,  A.  238.  108.) 

Zinc  molybdite,  Zn2Mo3O8  =  2ZnO,  3MoO2. 

Easily  sol.  in  aqua  regia.  (Muthmann,  A. 
238.  108.) 

Molybdovanadates. 
See  Vanadiomolybdates. 

Neodymicotungstic  acid. 

Ammonium  neodymicotungstate,  3(NH4)2O, 

Nd2O3,  16WO3+20H2O. 
Difficultly  sol.  in  H2O.     (E.  F.  Smith,  J. 
Am.  Chem.  Soc.  1904,  26.  1480.) 

Barium  neodymicotungstate,  6BaO,   Nd2O3, 

16WO3+17H2O. 
Insol.  in  H2O.    (E.  F.  Smith.) 

Neodymium. 

See  also  under  Didymium. 

Neodymium  bromide,  NdBr3. 

(Matignon,  C.  R.  1905,  140.  1638.) 

Neodymium  carbide,  NdC2. 

Decomp.  by  H2O;  insol.  in  cone.  HNO3; 
decomp.  by  dil.  HNO3.  (Moissan,  C.  R. 
1900,  131.  597.) 

Neodymium  chloride,  NdCl3. 

100  g.  H2O  dissolve  98.68  g.  NdCl3  at  13°; 
140.4  g.  at  100°. 

Sp.  gr.  at  15°/4°  of  the  solution  sat.  at  13°  = 


(Matignon,  A.  ch.  1906,  (8)  8.  249.) 


Bp. 

1.74. 

44.5  g.  are  sol.  in  100  g.  abs.  alcohol  at  20°. 
1.8  g.  "  "  "  "  pyridine  at  15°. 

Insol.  in  ether,  CHC13,  quinoline,  toluidine, 
etc.  SI.  sol.  in  aniline  and  in  phenylhydra- 
zine.  (Matignon,  A.  ch.  1906,  (8)  8.  266.) 

+6H2O.    Deliquescent. 

At  13°,  100  pts.  H2O  dissolve  246.2  pts.  of 
the  hydrated  salt. 

At  100°,  100  pts.  H2O  dissolve  511  pts.  of 
hydrated  salt. 

Sat.  solution  at  13°  has  a  sp.  gr.  15°/4°  = 
1.741.  (Matignon,  C.  R.  1901,  133.  289.) 

Neodymium     chloride     ammonia,     NdCl3. 

12NH3. 

Decomposes  on  heating  into  NdCl8+NHj; 
+2NH3;  +4NH8;  +5NH3;  +8NH3;  and 
+11NH8.  (Matignon,  C.  R.  1906, 142. 1043.) 

Neodymium  hydroxide. 

Sol.  in  citric  acid.  (Baskerville,  J.  Am. 
Chem.  Soc.  1904,  26.  49.) 


536 


NEODYMIUM  HYDRIDE 


Solubility  in  glycerine  -fAq  containing 
about  60%  by  vol.  of  glycerine.  100  ccm. 
of  the  solution  contain  4.5  g.  neodymium 
oxide.  (Miiller,  Z.  anorg.  1905,  43.  322.) 

Neodymium  hydride,  NdH2  (?). 

Slowly  attacked  by  boiling  H2O.  Sol.  in 
acids  with  violent  evolution  of  H2.  (Muth- 
mann,  A.  1904,  331.  58.) 

Neodymium  iodide,  NdI3. 

(Matignon,  C.  R.  1905,  140.  1638.) 

Neodymium  nitride,  NdN. 

Decomp.  in  moist  air  with  evolution  of 
NH3.  (Muthmann,  A.  1904,  331.  59.) 

Neodymium  oxide,  Nd2O3. 

Easily  sol.  in  acids,  (v.  Welsbach,  M.  6. 
477.) 

Neodymium  oxychloride,  NdOCl. 
(Matignon,  C.  R.  1905,  140.  1638.) 

Neon,  Ne. 

Less  sol.  than  argon  in  H2O;  sol.  in  liquid 
oxygen.  (Ramsay,  B.  1898,  31.  3118.) 

Absorption  by  H2O  at  t°. 


0 
10 
20 
30 
40 
50 


Coefficient  of  absorption 


0.0114 
0.0118 
0.0147 
0.0158 
0.0203 
0.0317 


(Antropoff,  Roy.  Soc.  Proc.  1910,  83.  A,  480.) 

Nickel,  Ni. 

Not  attacked  by  H2O.  Very  slowly  sol.  in 
dilute  H3PO4,  H2SO4,  or  HCl+Aq.  (Tup- 
puti,  A.  ch.  78.  133.) 

Very  easily  attacked  by  HNO3+Aq,  and 
difficultly  by  hot  H2SO4.  When  pure,  is  con- 
verted into  passive  condition  by  cone.  HNO3. 
(Nickles,  C.  R.  38.  284.) 

Very  si.  attacked  by  cold  acids,  except 
HNO3+Aq.  (Tissier,  C.  R.  60.  106.) 

Not  attacked  by  NaOH+Aq.  (Venator, 
Dingl.  261.  133.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 

Nickel  amide,  Ni(NH2)2. 

Decomp.  by  H2O;  slowly  sol.  in  min.  acids. 
Insol.  in  liquid  NH3.  (Bohart,  J.  phys.  Chem. 
1915,  19.  560.) 

Nickel  antimonide,  NiSb. 

Insol.  in  HCl+Aq;  easily  sol.  in  HNO3  + 
Aq.  (Christofle,  1863.) 


Min.  Breithauptite.     Insol.  in  acids;  easily 
sol.  in  aqua  regia. 
Ni3Sb2.    (Christofle.) 

Nickel  antimonide  sulphide,  NiSb2,  NiS2  = 
NiSbS. 

Min.  Nickel  glance,  Ullmannite. 

Decomp.  by  HNO3+Aq;  completely  sol. 
in  aqua  regia  with  separation  of  S. 

Nickel  arsenide,  NiAs. 

Min.  Niccolite.  Sol.  in  cone.  HNO3+Aq 
with  separation  of  As2O3;  more  easily  sol.  in 
aqua  regia. 

NiAs2.  Min.  Chloanthite,  Rammelsbergite. 
Sol.  in  HNO3+Aq. 

Ni3As2.  Sol.  in  HNO3  and  in  aqua  regia. 
Readily  attacked  by  fused  alkali.  (Granger, 
C.  R.  1900,  130.  915.) 

Nickel  arsenide  sulphide,  NiAs2,  NiS2. 

Min.  Gersdorffite.  Partly  sol.  in  HN03  + 
Aq  with  separation  of  S  and  As2O3;  not  at- 
tacked by  KOH+Aq. 

Nickel  azoimide,  basic,  Ni(OH)N3 

Insol.  in  H2O.  (Curtius,  J.  pr.  1898,  (2) 
58.  300.) 

Nickel  azoimide,  NiN6+H2O. 

Sol.  in  H2O;  insol.  in  alcohol  and  ether. 
(Curtius,  J.  pr.  1900,  (2)  61.  418.) 

Nickel  potassium  azoimide,  Ni(N3)2,  KN3  (?). 
Sol.  in  H2O.    (Curtius,  J.  pr.  1898,  (2)  58. 
302.) 

Nickel  boride,  Ni2B. 

Attacked  by  HNO3.  Slowly  sol.  in  hot 
HC1.  (Jassoneix,  C.  R.  1907,  145.  240.) 

NiB.  Decomp.  by  moist  air  and  by  alkali 
nitrates,  chlorates,  hydroxides  and  carbon- 
ates; decomp.  by  steam  at  red  heat.  Not 
attacked  by  HC1.  Easily  attacked  by  HNO3 
and  aqua  regia;  by  H2S04  only  on  heating. 
(Moissan,  C.  R.  1896,  122.  425.) 

NiB2.    (Jassoneix,  C.  R.  1907,  145.  241.) 

Nickel  bromide,  NiBr2. 

Deliquescent.    Slowly  sol.  in  H2O. 

Sat.  NiBr2+Aq  contains  at: 
—21°      —6°       +19°       38° 
47.1        51.7        56.6        58.9%  NiBr2, 

58°         77°         98°        100°       140° 
60.5       60.3       61.0       61.0       60.7%  NiBr2. 
(Etard,  A.  ch.  1894,  (7)  2.  542.) 

Somewhat  hygroscopic.  Nearly  insol.  in 
cold  H2O  but  begins  to  dissolve  appreciably 
at  50°,  and  somewhat  more  rapiotly  at  90°, 
but  even  at  that  temp.  1  g.  requires  1-2  hours 
for  solution.  HNO3  does  not  appreciably 
hasten  solution.  (Richards  and  Cushman, 
Z.  anorg.  1898,  16.  169.) 


NICKEL  CHLORIDE 


537 


SI.  sol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1369.) 

Sol.  in  quinoline.  (Beckmann  and  Gabel, 
Z.  anorg.  1906,  61.  236.) 

+3H2O.  Deliquescent.  Very  sol.  in  H20, 
HCl+Aq,  NH4OH+Aq,  alcohol,  and  ether. 
(Berthemot,  A.  ch.  44.  389.) 

+6H2O.  (Bolschakoff,  C.  C.  1897,  II. 
331  and  726.) 

+9H2O.  (Bolschakoff,  C.  C.  1897,  II. 
726  and  331.) 

Nickel  stannic  bromide. 
See  Bromostannate,  nickel. 

Nickel  bromide  ammonia,  NiBr2,  6NH6. 

Sol.  in  little  H2O,  but  decomp.  by  more. 
(Rammelsberg,  Pogg.  55.  243.) 

Sol.  in  warm  cone.  NH4OH+Aq;  insol.  in 
cold.  (Richards  and  Cushmann,  Z.  anorg. 
1898,  16.  175.) 

Nickel  bromide  cupric  oxide,  NiBr2,  3CuO  + 

4H2O. 

Not  decomp.  by  H2O.  (Mailhe,  A.  ch. 
1902,  (7)  27.  377.) 

Nickel  bromide  hydrazine,  NiBr2,  2N2H4. 

Easily  sol.  in  dil.  acids  and  NH4OH+Aq. 

NiBr2,  3N2H4.  Sol.  in  dil.  acids.  (Franzen, 
Z.  anorg.  1908,  60.  263-4.) 

Nickel  carbonyl,  Ni(CO)4. 

Insol.  in  H2O;  not  attacked  by  dil.  acids  or 
alkalies  or  cone.  HCl+Aq.  Easily  sol.  in 
cone.  HNOs+Aq  and  in  aqua  regia.  Sol.  in 
alcohol,  benzene,  and  chloroform.  (Mond, 
Langer,  and  Quincke,  Chem.  Soc.  57.  749.) 

Sol.  in  hydrocarbons,  especially  oil  of  tur- 
pentine. (Berthelot,  C.  R.  1891,  112.  1346.) 

Sol.  in  acetone,  toluene,  methyl  and  ethy] 
alcohol,  etc.  (Lenher  and  Loos,  J.  Am.  Chem 
Soc.  1900,  22.  114.) 

Nickel  chloride,  NiCl2. 

Anhydrous.  Not  immediately  sol.  in  H2O 
but  gradually  dissolves  on  boiling  or  by  addi- 
tion of  HCl+Aq.  Deliquesces  on  air,  and  is 
then  easily  sol.  in  H2O.  Sol.  in  NH4OH+Aq. 
Sol.  in  alcohol.  Sol.  in  hot  HCl+Aq  only 
slowly. 

Sp.  gr.  of  NiCl2+Aq  containing: 
5          10          15          20          25%  NiCl2 
1.0493    1.0995    1.1578    1.2245    1.3000 
(B.  Franz,  J.  pr.  (2)  6.  285.) 


Sp.  gr.  of  NiCl2+Aq  containing, 
grms.  H2O,  g.  NiCl2+7H2O  at  23.1°: 

128  g.  ( =  Y2  mol.)     256       384       512 
1.057  1.107     1.149 

640       768       896       1024 
1.220     1.249     1.276     1.301 


in  100C 


1.187 


Hontaining  g.  NiCl2  (anhydrous) : 
65  g.  (  =  Y2  mol.)  130*  195     260     325     390 
1.061  1.119  1.176  1.230  1.284  1.335 

(Gerlach,  Z.  anal.  28.  468.) 

Sp.  gr.  of  NiCl2+Aq  at  room  temp,  con- 
aining : 

11.449       22.69       30.40%  Ni.Cl2. 
1.1093       1.2264       1.3371 
(Wagner,  W.  Ann.  1883,  18.  269.) 

Sp.  gr.  of  NiCl2+Aq  at  25°. 


Concentration  of  NiCb+Aq 


1-normal 

Vr-      " 


V 


Sp.  gr. 


1.0591 
1.0308 
1.0144 
1.0067 


(Wagner,  Z.  phys.  Ch.  1890,  5.  39.) 

Insol.  in  liquid  NH3.  (Franklin,  A.m.  Ch. 
J.  1898,  20.  828.) 

100  pts.  absolute  alcohol  dissolve  at  room 
temperature  10.05  pts.  NiCl2.  (Bodtker,  Z. 
phys.  Ch.  1897,  22.  511.) 

Sol.  in  quinoline.  (Beckmann  and  Gabel, 
Z.  anorg.  1906,  51.  236.)  < 

Difficultly  sol.  in  methyl  acetate.  (Nau- 
mann,  B.  1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

Solubility  in  glycol  =  16. 1-16.3%.  (de 
Coninck,  C.  C.  1905,  II.  1234.) 

SI.  sol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1369.) 

Anhydrous  NiCl2  -is  insol.  in  acetone. 
(Krug  and  M'Elroy,  J.  Anal.  Ch.  6.  184.) 

Insol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

+H2O.    (Baubigny.) 

1 1.  sat.  HCl+Aq  at  12°  contains  40  g.  NiCl2 
dissolved  from  NiCl2,  H2O.  (Ditte.) 

+2H2O.    (Sabatier,  Bull.  Soc.  (3)  1.  88.) 

+6H2O.  Deliquescent  in  moist,  efflores- 
cent in  dry  air;  sol.  in  H2O  with  evolution  of 
heat.  Sol.  in  1.5  to  2  pts.  H2O.  Easily  sol. 
in  alcohol.  (Tupputi.) 

1  1.  H2O  dissolves  600  g.  NiCl2+6H2O. 
(Ditte,  A.  ch.  1879,  (5)  22.  551.) 

Sat.  aq.  solution  contains  at: 
—17°  —16°  +10°  18° 
29.7  31.0  37.3  38.5%  NiCls, 

38°        59°        78°        96° 
41.9       45.0       46.6      46.7%  NiCl2. 
(fitard,  A.  ch.  1894,  (7)  2.  539.) 

Solubility  of  NiCl2+6H2O  =  37.53%  NiCl2 
at  25°.  (Foote,  J.  Am.  Chem.  Soc.  1912,  34. 
882.) 

100  pts.  absolute  alcohol  dissolve  at  room 
temperature  53.71  pts.  NiCl2+6H2O.  (Bodt- 
ker, Z.  phys.  Ch.  1897,  22.  511.) 


538 


NICKEL  HYDROGEN  CHLORIDE 


+7H2O.  100  g.  absolute  alcohol  dissolv 
2.16  g.  NiCl2+7H2O  at  17°  and  1.4  g.  at  3° 
(de  Bruyn,  R.  t.  c.  1892,  11.  156.) 

Nickel  hydrogen  chloride,  3NiCl2,  2HC1+ 

1^H2O. 
(Reitzenstein,  Z.  anorg.  1898,  18.  270.) 

Nickel  rubidium  chloride,  NiCl2,  2RbCl. 

Easily  sol.  in  H2O  and  HCl+Aq.  (Godef- 
froy,  B.  8.  9.) 

Nickel  thallic  chloride,  NiCl2,  2T1C13+8H2O 

Deliquescent.     Can  be  cryst.  from  H2O. 

(Gewecke,  A.  1909,  366.  221.) 

Nickel  tin  (stannous)  chloride,  NiCl2,  SnCl2+ 

6H2O. 
Sol.  in  H2O.    (Jorgensen.) 

Nickel  tin  (stannic)  chloride. 
See  Chlorostannate,  nickel. 

Nickel  chloride  ammonia,  NiCl2,  2NH3. 

Sol.  in  H2O,  decomp.  on  boiling;  insol.  in 
alcohol. 

NiCl2,  3NH3+3H2O.  (Andre,  C.  R.  1888, 
106.  937.) 

NiCl2,  6NH3.  Sol.  in  cold  H2O  without 
decomp.  Insol.  in  alcohol.  Very  si.  sol.  in 
cone.  NH4OH+Aq. 

Nearly  insol.  in  a  sat.  solution  of  NH4C1 
in  NH4OH+Aq.  (Sorensen,  Z.  anorg.  1894, 
5.  363.) 

Nickel  chloride  cupric.  oxide,  NiCl2,  3CuO  + 

4H2O. 

Not  decomp.  by  H2O.  (Mailhe,  A.  ch. 
1902,  (7)  27.  377.) 

Nickel  chloride  hydrazine,  NiCl2,  2N2H4. 

Sol.  in  dil.  acids  and  NH3+Aq.  (Franzen, 
Z.  anorg.  1908,  60.  262.) 

NiCl2,  3N2H4.    Sol.  in  dil.  acids.    (F.) 


Nickel  potassium  fluoride,  NiF2,  KF. 

+H2O.     Sol.  in  H20.     (Wagner,   B.   19. 
896.) 


NiF2,  2KF.  SI.  sol.  in  H2O. 
in  methyl  or  ethyl  alcohol 
(Poulenc,  C.  R.  114.  747.) 


Scarcely  sol. 
,  or    benzene. 


Nickel  potassium  zirconium  fluoride. 
See  Fluozirconate,  nickel  potassium. 

Nickel  manganic  fluoride. 
See  Fluomanganate,  nickel. 

Nickel  sodium  fluoride,  NiF2,  NaF-fH2O. 
Sol.  in  H2O.    (Wagner,  B.  19.  896.) 

Nickel  stannic  fluoride. 
See  Fluostannate,  nickel. 

Nickel  titanium  fluoride. 
See  Fluotitanate,  nickel. 

Nickel  tungstyl  fluoride. 
See  Fluoxytungstate,  nickel. 

Nickel  vanadium  fluoride. 
See  Fluovanadate,  nickel. 

Nickel  zirconium  fluoride. 
See  Fluozirconate,  nickel. 

Nickel    fluoride    ammonia,   5NiF2,    6NH3  + 

8H2O. 

Insol.  in  cold  H2O.  Decomp.  by  hot  H2O. 
Easily  sol.  in  dil.  acids.  (Bohm.  Z.  anorg. 
1905,  43.  334.) 

Nickelous  hydroxide,  4NiO2H2,  H2O. 

-Very  si.  sol.  in  H2O.  Sol.  in  acids.  Insol. 
in  KOH  or  NaOH+Aq.  Somewhat  diffi- 
cultly sol.  in  (NH4)2CO3  or  NH4OH+Aq,  but 
easily  sol.  in- presence  of  NH4  salts.  Sol.  in 
NH4  salts+Aq.  Sol.  in  KCN+Aq.  (Rod- 
gers,  1834.) 

Sol.  in  boiling  NH4Cl+Aq. 


Nickel  fluoride,  NiF2. 
Sol.  in  about  5000  pts.  H2O;  insol.  in  alcohol 
and  ether.    Not  attacked  by  HC1,  HNO3,  or 
H2SO4  even  when  hot.    (Poulenc,  C.  R.  114. 
1426.) 
Insol.  in  liquid  NH3.     (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 
+2H2O.    Decomp.  by  pure  H2O.    Sol.  in 
H2O  acidulated  with  HF.    (Berzelius.) 
+3H2O.    (Clarke,  Sill.  Am.  J.  (3)  13.  291.) 

Nickel  hydrogen  fluoride,  NiF2,  5HF+6H2O. 
Easily  sol.  in  H2O  and  dil.  acids.    Sol.  in 
NH4OH+Aq    with    decomp,       (Bohm,    Z. 

n-nn-nrr      1  Qfl£      AQ      QQfl   "> 

Ni02H2. 
Solubility  in  NH4OH+Aq  at  25°. 

NHs  norm. 

G.  Ni  per  1. 

G.  Ni02H2  per  1. 

1 

2 
3 

4 

0.084 
0.170 
0.257 
0.360 

0.00287 
0.00579 
0.00875 
0.01227 

4.911 
3.900 
2.101 
0.602 

2.580 
1.780 
0.835 
0.158 

0.0879 
0.0607 
0.0284 
0.0054 

;he  formation  of  different  modifications  of 
NiO2H2. 

(Bonsdorff,  Z.  anorg.  1904,  41.  185.) 


NICKEL  PHOSPHIDE 


539 


Solubility  in  NH4OH+Aq. 

Cone,  of  Ni  =  0.014N  in  IN  NH4OH+Aq. 
"     "   "  =0.036N  "2NNH4OH+Aq. 

CStarck,  B.  1903,  36.  3840.) 

Sol.  in  hot  NH4F+Aq.  (von  Helmolt,  Z. 
anorg.  1893,  3.  133.) 

Insol.  in  methyl  or  amyl  amine.    (Wurtz.) 

Not  pptd.  in  presence  of  Na  citrate. 
(Spiller.) 

Not  pptd.  in  presence  of  a  large  number  of 
non-volatile  organic  substances,  particularly 
H2C4H4O6.  (Rose.) 

Nickelonickelic  hydroxide,  Ni3O4,  2H2O. 

Sol.  in  acids;  insol.  in  H2O  and  alkalies. 
(Dudley,  J.  Am.  Chem.  Soc.  1896,  18.  901.) 

Nickelic  hydroxide,  Ni2O3,  2H2O  (?). 

(Wernicke,  Pogg.  141.  122.) 

Ni2O3,  3H2O  (?).  Sol.  in  acids  as  nickelous 
salts.  Not  attacked  by  boiling  KOH  or 
NaOH+Aq.  Slowly  sol.  in  HC2H3O2+Aq. 
Sol.  in  NH4OH,  and  NH4  salts+Aq.  (Od- 
ling.) 

Nickel  iodide,  NiI2. 

Deliquescent  and  sol.  in  H2O.  (Erdmann, 
J.  pr.  7.  254.) 

Sat.  NiI2+Aq  contains  at: 
—23°      —6°       +11°        16° 
51.8        54.3        57.8        59.0%  NiI2, 

43°          80°        85°         90° 
64.1        65.0        65.2        65.7%  NiI2. 
(Etard,  A.  ch.  1894,  (7)  2.  546.) 

+6H2O.  Deliquescent.  Easily  sol.  in 
H2O.  (Erdmann.) 

Nickel  iodide  ammonia,  NiI2,  4NH3. 

(Rammelsberg,  Pogg.  48.  119.) 

NiI2,  6NH3.  Decomp.  by  H2O.  Sol.  in 
warm  oil.  NH4OH+Aq.  Very  si.  sol.  in  cone. 
NH4OH+Aq.  (Erdmann.) 

Nickel  iodide  hydrazine,  NiI2(N2H4)2. 

Insol.  in  H2O.  Sol.  in  acids.  (Franzen, 
Z.  anorg.  1911,  70.  150.) 

Nickel  sutoxide,  Ni3O2+H2O. 

Insol.  in  H2O;  sol.  in  HC1  and  H2SO4  and 
HNO3;  also  in  KCN+Aq.  (Moore,  C.  N. 
1895,  71.  81.) 

Nickelous  oxide,  NiO. 

Insol.  in  H2O.  Sol.  in  cone,  acids,  except 
when  crystalline,  when  it  is  scarcely  attacked 
by  acids.  (Ebelmen,  C.  R.  33.  256.) 

Very  si.  sol.  in  boiling  NH4Cl+Aq.  (De- 
margay.) 

Very  slowly  sol.  in  NH4OH+Aq.  Insol.  in 
KOH,  and  NaOH+Aq. 

Sol.  in  min.  acids,  especially  HCl+Aq, 
when  warmed;  insol.  in  HC2H3O2,  NH4C1, 


and  NH4SCN+Aq.  Insol.  in  cone.  NaOH+ 
Aq.  (Zimmerman,  A.  232.  324.) 

1  1.  solution  containing  418.6  g.  sugar  and 
34.3  g.  CaO  dissolves  0.29  g.  NiO.  (Boden- 
bender,  J.  B.  1866.  600.) 

Min.  Bunsenite. 

Nickelonickelic  oxide,  Ni304. 

Sol.  in  acids.    (Baubigny,  C.  R.  87.  1082.) 
+2H2O.    Insol.  in  H2O,  and  in  alkalies+ 

Aq.    Sol.  in  acids.     (Dudley,  J.  Am.  Chem. 

Soc.  1896,  18.  901.) 

6NiO,  Ni2O3+H2O.    (Schonbein,  J.  pr.  93. 

35.) 

Nickelic  oxide,  Ni2O3. 

Sol.  in  HNO3,  H2SO4,  or  HCl+Aq  with 
decomp.,  also  in  NH4OH  and  (NH4)2CO3  + 
Aq.  (Winkelblech,  A.  13.  259.) 

Nickel  peroxide,  Ni3O6  (?). 

(Bayley,  C.  N.  39.  81.) 

Correct  composition  is  Ni2O3.  (Carnot, 
C.  R.  108.  610.) 

Ni4O7  (?).    (Wicke,  Zeit.  Ch.  1865.  303.) 

NiO4.    (Hollard,  C.  R.  1903,  136.  230.) 

Nickel  oxychloride. 

SI.  sol.  in  H2O.    (Berzelius.) 

NiCl2,  8NiO+13H2O.    (Raoult,  C.  R.  69. 


Nickel  oxyiodide,  NiI2,  9NiO  +  15H2O. 

Insol.  in  H2O.  Sol.  in  HNO3+Aq  or  acetic 
acid.  Insol.  in  NH4OH+Ac*.  Alcohol  dis- 
solves out  NiI2.  (Erdmann.) 

Nickel  oxyselenide. 

Ahnost  insol.  in  boiling  HC1;  decomp.  by 
HNO3.  (Fonzes-Diacon,  C.  R.  1900,  131. 

557.) 

Nickel  phosphide,  Ni2P. 

Sol.  in  HNO3+Aq  and  aqua  regia;  insol.  in 
HCl+Aq.  (Struve,  J.  pr.  79.  321.) 

Sol.  in  aqua  regia  and  in  HNO3;  sol.  in 
fused  alkali.  (Granger,  Bull.  Soc.  1896,  (3) 
15.  1089.) 

Easily  sol.  in  HN03.  (Granger,  C.  N.  1898, 
77.  229.) 

When  prepared  by  heating  phosphorus, 
copper  and  nickel  in  electric  furnace,  is  insol. 
in  all  acids  except  a  mixture  of  HNO8  and 
HF.  (Maronneau,  C.  R.  1900,  130.  657.) 

NiP2.  Sol.  in  HNO3;  decomp.  by  fused 
NaOH.  (Jolibois,  C.  R.  1910,  150.  107.) 

NiP3.  Sol.  in  HNO3;  decomp.  by  fused 
NaOH.  (J.) 

Ni2P3.  Insol.  in  HNO3,  HC1  and  aqua 
regia;  stable  in  the  air  even  when  heated 
(Granger,  Bull.  Soc.  1896,  (3)  15.  1086.) 

Ni3P2.  Not  attacked  by  HC1.  Easily  at- 
tacked by  HNO3.  (Rose,  Pogg.  1832^  24. 
232.) 


540 


NICKEL  PHOSPHOSULPHIDE 


N5P2.  Sol.  in  HNO3,  aqua  regia  and  in 
fused  alkali.  (Granger,  C.  R.  1896,  123.  177. 

Nickel  phosphosulphide,  Ni3PS3. 

Decomp.  by  hot  H2O  or  by  aqua  regia 
SI.  attacked  by  HNO3.  (Ferrand,  A.  ch 
1899,  (7)  17.  417.) 

Nickel  semiselenide,  Ni2Se. 

Almost  insol.  in  boiling  HC1;  decomp.  by 
HNO3.  (Fonzes-Diacon,  C.  R.  1900,  131. 

557.) 

Nickel  selenide,  NiSe. 

Insol.  in  H2O,  dil.  or  cone.  HCl+Aq 
slowly  sol.  in  HNO3+Aq;  easily  in  aqua  regia 
(Little,  A.  112.  211.) 

Almost  insol.  in  boiling  HC1;  decomp.  by 
HNO3.  (Fonzes-Diacon,  C.  R.  1900,  131. 
557.) 

NiSe2.    (Fonzes-Diacon.) 

Ni3le43j  Almosfc  inso1-  in  boiling  HC1; 
decomp.  by  HNO3.  (Fonzes-Diacon.) 

Nickel  siHcide,  Ni2Si. 

Sol.  in  HF  and  aqua  regia;  insol.  in  cold 
H2O;  decomp.  by  steam  at  red  heat;  sol.  in 
fused  alkali  carbonates.  (Vigouroux,  C.  R. 
1895,  121.  687.) 

Nickel  semzsulphide,  Ni2S. 

Sol.  in  HNp3+Aq,  with  residue  of  S. 
Difficultly  sol.  in  cone.  HCl+Aq;  insol.  in 
dil.  HCl+Aq.  (Arfvedson,  Pogg.  1.  65; 
Gautier,  C.  R.  108.  1111.) 

Does  not  exist.  (Bornemann,  C.  A.  1908. 
1686.) 

Nickel  raonosulphide,  NiS. 

Anhydrous.  Insol.  in  H2O,  HC1,  or  H2SO4 
+Aq.  Sol.  in  HNO3+Aq  or  aqua  regia. 

Min.  Millerite. 

+rcH2O.  Insol.  in  H2O,  but  decomp.  by 
H2O  in  contact  with  the  air  (Clermont  and 
Guiot,  C.  R.  84.  714),  or  by  boiling  with  H2O. 
(Geitner,  A.  139.  354.) 

When  pptd.  with  (NH4)2S,  is  somewhat  sol. 
in  H20.  1  1.  H2O  dissolves  39.87  X 10  6  moles 
NiS  at  18°.  (Weigel,  Z.  phys.  Ch.  1907,  68. 
294.) 

Very  si.  sol.  in  dil.  HCl+Aq,  and  still  less 
in  HC2H3O2+Aq.  (Fresenius.) 

More  sol.  in  HNO3+Aq,  and  easily  in  aqua 
regia. 

Somewhat  sol.  in  NH4OH+Aq  or  solutions 
of  alkali  sulphides.  Insol.  in  NH4SH+Aq. 
(Fresenius.) 

Sol.  at  moment  of  formation  in  Na2S  but 
not  in  (NH4)2S+Aq.  (Villiers,  C.  R.  1894, 
119.  1264.) 

Sol.  while  yet  moist  in  H2SO3+Aq.  (Ber- 
thier.) 

When  recently  pptd.,  sol.  in  KCN+Aq. 
(Haidlen.) 


Pptd.  in  presence  of  non- volatile  organic 
substances  as  tartaric  acid,  etc.  (Rose.) 

Sol.  in  potassium   thiocarbonate+Aq. 
(Rosenbladt,  Z.  anal.  26.  15.) 

Exists  in  a  colloidal  form  in  a  very  dil. 
solution.  (Winnsinger,  Bull.  Soc.  (2)  49.  452.) 

a  modification: 

Very  sol.  in  2N-HCl+Aq  sat.  with  H2S. 

j8  modification: 

0.033  g.  is  sol.  in  1  1.  2N-HCl+Aq  sat. 
with  H2S;  very  sol.  in  2N-HCl+Aq. 

7  modification: 

Insol.  in  2N-HCl+Aq  sat.  with  H2S. 
0.013  g.  is  sol.  in  2N-HCl+Aq.  (Thiel, 
C.  C.  1914,  I.  19.) 

Nickel  sulphide,  Ni3S2, 

(Bornemann,  C.  A.  1908.  1686.) 

Ni3S4.    (Bornemann.) 

Ni6S6.    (Bornemann.) 

Ni4S5.  Min.  Polydymite.  Insol.  in  HC1+ 
Aq.  Sol.  in  HNO3+Aq  with  separation  of  S. 

Ni5S7.    Min.  Beyrichite.    Sol.  in  HCl+Aq. 

Nickel  bisulphide,  NiS2. 
(Fellenberg,  Pogg.  50.  75.) 
Does  not  exist.    (Bellucci,  C.  A.  1909.  293.) 

Nickel  potassium  sulphide,  3NiS,  K2S. 

Insol.  in  H2O.     (Schneider,  J.   pr.  (2)  9. 

EsNiiiSio.  Not  attacked  by  hot  (NH4)2S; 
slowly  attacked  by  HC1  or  cold  aqua  regia; 
quickly  by  hot  aqua  regia.  HF  and  H2SQ4 
dissolve  only  on  heating.  Insol.  in  organic 
acids,  alkalies  and  12%  HC1,  also  in  KCN, 
AgNO3  or  CuSO4+Aq.  (Milbauer,  Z.  anorg. 
1904,  42.  447.) 

Nickel  telluride,  Ni2Te3. 

Min.  Melonite.    Sol.  in  HN03+Aq. 
NiTe.    (Fabre,  C.  R.  105.  277.) 

Nickelicotungstic  acid. 

Ammonium  nickelicotungstate,  2(NH4)2O, 
.2Ni2O3,  8WO3+14H2O. 

(Rogers  and  Smith,  J.  Am.  Chem.  Soc. 
1904,  26.  1476.) 

3(NH4)20,  Ni203,  16W03+22H20.  Very 
si.  sol.  in  H2O.  (Rogers  and  Smith.) 

Barium  nickelicotungstate,    19BaO,     Ni2O3, 

16W03. 
Ppt.    Very  insol.  in  H2O.    (E.  F.  Smith.) 

STickelimolybdic  acid. 

Barium   nickelimolybdate,    3BaO,    NiO2, 

9MoO3  +  12H2O. 
Ppt.     (Hall,  J.  Am.  Chem.  Soc.  1907,  29. 

02.) 


NITRATOPURPUREOCOBALTIC  BROMIDE 


541 


Potassium    nickelimolybdate,    3K2O,    NiO2, 

9MoO3+63^H2O. 
Very  insol.  even  in  hot  H2O.    (Hall.) 

Nickelomolybdic  acid. 

Ammonium  hydrogen  nickelomolybdate, 

(NH4)4H6[Ni(MoO4)6]  +5H2O. 
SI.  sol.  in  H2O,  easily  in  dil.  acids.     (Bar- 
bieri,  C.  A.  1915.  897.) 

Barium  hydrogen  nickelomolybdate, 

Ba2H6[Ni(MoO4)6]  +  10H2O. 
Ppt.    (Barbieri.) 

Potassium  hydrogen  nickelomolybdate. 
K4H6[Ni(Mo04)6]+5H20. 
SI.  sol.  in  H2O,  easily  in  acids.    (Barbieri.) 

Silver  hydrogen  nickelomolybdate, 

Ag4H6[Ni(Mo04)6]+3H20. 
Insol.  in  H2O;  sol.  in  NH4OH,  or  HNO3+ 
Aq.    (Barbieri.) 

Nickelonickelous  acid. 

Potassium  nickelonickelite,  K2Ni2O4  or  K2O, 

NiO,  NiO2. 

'(Hofmann  and  Hiendlmaier,  B.  1906,  39. 
3186.) 

Sodium   nickelonickelite,    Na2  Ni3O6  =  Na2O, 

NiO,  2NiO2. 
(Bellucci  and  Rubegni,  C.  C.  1907, 1.  794.) 

Nickelous  acid. 

Barium  eftnickelite,  BaO,  2NiO2. 

Unstable;  decomp.  by  cold  H2O;  slowly 
and  very  rapidly  by  hot  H2O.  (Dufau,  C.  R. 
1896,  123.  496.) 

Niobium,  Nb. 

For  niobium  and  its  compounds,  see  colum- 
bium,  Cb,  and  the  corresponding  compounds. 

Nitramide,  NH2NO2. 

Decomp.  by  cone.  H2S04.  Easily  sol.  in 
H2O,  alcohol, 'ether  and  acetone.  Less  sol.  in 
benzol.  Almost  insol.  in  ligroin.  (Thiele  and 
Lachman,  A.  1895,  288.  297.) 

Sol.  in  ether,  insol.  in  petroleum  ether. 
Very  unstable;  decomp.  by  hot  H2O.  (Thiele 
and  Lachman,  B.  1894,  27.  1909.) 

Nitratochloroplatinamine  comps. 
See  Chloronitratoplatinamine  comps. 

Nitratocobalt  octamine  comps. 
See  Nitratooctamine  cobaltic  comps. 


Nitratooctamine  cobaltic  carbonate, 

(N03)2Co2(NH3)8(C03)2+H20. 
Less  sol.  than  other  octamine  carbonates. 
(Vortmann  and  Blasberg,  B.  22.  2650.) 

chloride,  (NO3)2Co2(NH3)8Cl4+4H2O. 

(Vortmann  and  Blasberg,  B.  22.  2652.) 

iodide,  (NO3)2Co2(NH3)8I4+2H2O. 

(Vortmann  and  Blasberg.) 

nitrate. 

See  Octamine  cobaltic  nitrate. 

sulphate,    (N03)2Co2(NH3)8(S04)2  + 

2H20. 
+4H2O.    (Vortmann  and  Blasberg,  B.  22. 

2652.) 

Nitratoplatinarnine  nitrate, 

(N03)2Pt(NH3N03)2. 

SI.  sol.  in  cold,  more  easily  in  hot  H2O; 
easily  sol.  in  dil.  HNO3+Aq.    (Cleve.) 

nitrite,  (NO,),Pt(NH,NO,),. 

Easily  sol.  in  H2O.    (Cleve.) 

Nitratoplatindiamine  chloride, 

(NO3)2Pt(N2H6Cl)2+H2O. 
Moderately  sol.  in  cold,  very  easily  in  hot 
H2O. 

—  chloroplatinate,    (NO3)2Pt(N2H6Cl)2, 
PtCl4+2H2O. 

Ppt. 

—  chromate,  (NO3)2Pt(N2H6)2CrO4. 
Nearly  insol.  in  H2O.    (Cleve.) 

^chromate,  (NO3)2Pt(N2H6)2Cr2O7. 

SI.  sol.  in  H2O. 


nitrate,  (NO3)2Pt(N2H6NO3)2. 

Sol.  in  H2O.    Insol.  in  HNO3+Aq. 

phosphate,  NO3Pt(N2H6)2+H2O. 

\   / 
P04 
Very  si.  sol.  in  H2O.    (Cleve.) 

Nitratodi'platindiamin  e  nitrate, 

(N03)2Pt2(N2H6)4(N03)4. 
Sol.  in  H2O  with  decomp. 

Nitratopurpureocobaltic  bromide, 

Co(NO3)(NH3)6Br2. 

Resembles  the   chloride  in  its  properties. 
(Jorgensen,  J.  pr.  (2)  23.  227.) 


542 


NITRATOPURPUREOCOBALTIC  CARBONATE 


Nitralopurpureocobaltic  carbonate, 

Co(N03)(NH3)5(C03)+H20. 
Less  sol.  in  H2O  than  other  purpureocar- 
bonates.     (Vortmann  and  Blasberg,  B.  22. 
2648.) 

—  chloride,  Co(NO3)(NH3)5Cl2. 

SI.  sol.  in  cold  H2O,  but  more  than  nitrate; 
more  easily  sol.  in  hot  H2O,  but  is  converted 
into  roseo  salt.  Insol.  in  HCl+Aq  or  alcohol. 
(Jorgensen,  J.  pr.  (2)  23.  227.) 

mercuric  chloride, 

Co(NO3)(NH3)5Cl2,  HgCl2. 
Not  wholly  insol.  in  H2O.     (Jorgensen.) 

chloroplatinate,    Co(NO3)(NH3)5Cl2, 

PtCl4. 

Ppt.  Nearly  insol.  in  cold  H2O.  (Jorgen- 
sen.) 


chromate,  Co(NO3)(NH3)5CrO4. 

Nearly  insol.  in  H2O.    (Jorgensen.) 

bichromate. 

SI.  sol.  in  H2O,  but  more  easily  than  the 
neutral  salt.  (Jorgensen.) 

dithionate,  Co(NO3)(NH3)5S2O6. 

Very  si.  sol.  in  cold,  more  easily  in  hot  H2O. 
(Jorgensen.) 

nitrate,  Co(NO3)(NH3)5(NO3)2. 

Sol.  in  273  pts.  H2O  at  16°.  Much  more  sol. 
in  hot  H2O  containing  HNO3.  (Jorgensen,  J. 
pr.  (2)  23.  227.) 

cobaltic  nitrite,  3Co(NO3)(NH3)5, 

2Co(NO2)6+2H2O. 

Very  si.  sol.  in  H2O.  (Jorgensen,  Z.  anorg. 
5.  176.) 

diamine  cobaltic  nitrite,  Co(NO3)(NH3)6 

(N02)4Co(NH3)2. 
Ppt.    (Jorgensen.) 

oxalate,  Co(NO8)(NH3)5C2O4. 

Ppt. 

sulphate,  Co(NO3)(NH3)5SO4+H2O. 

Rather  difficultly  sol.  in  cold  H2O.  (Jor- 
gensen.) 

Nitratopurpureorhodium  chloride, 

(NO3)Rh(NH3)5Cl2. 

SI.  sol.  in  cold  H2O,  but  more  easily  than 
the  nitrate.  (Jorgensen,  J.  pr.  (2)  34.  394.) 

-  dithionate,  (NO3)Rh(NH3)5S2O6+H2O. 
Nearly  insol.  in  cold  H2O.    (Jorgensen.) 


Nitratopurpureorhodium  nitrate, 

(NO3)Rh(NH3)5(NO3)2. 
Very  si.  sol.  in  cold  H2O.    Insol.  in  alcohol. 
(Jorgensen.) 

Nitric  acid,  HNO3. 

Miscible  with  H2O.  When  HNO3+Aq  is 
distilled  at  760  mm.  pressure,  an  acid  contain- 
ing 68%  HNO3  is  formed,  which  boils  at 
120.5°  under  735  mm.  pressure.  By  distilling 
at  150  mm.  pressure  the  acid  contains  67.6% 
HNO?;  at  70  mm.  (b.-pt.  65-70°)  the  acid 
contains  66.7%  HN03.  The  percentage  of 
HNO3  in  the  liquid  obtained  by  passing  dry 
air  into  HNO3+Aq  containing  64-68%  HNO3 
varies  with  the  temp.;  the  higher  the  temp, 
the  greater  the  percentage  of  HNO3.  (Roscoe, 
Chem.  Soc.  13.  150.) 

HNOs-trAq  of  1 .51     sp.  gr.  contains  67%  N2O6. 
142  "  "        54 

1.35  "  "        44.4 

1.315         "          •"        38.6 

(Dalton.) 

HNOs+Aq  of  1 .52    sp.  gr.  contains  88.82%  N2O5. 
1.522         "  "         86.17%      " 

1.4  "  "         44 

(Mitscherlich.) 

HNOs+Aq  of  1.298  sp.  gr.  contains  36.75%   N2OS. 

(Kirwan.) 

HNOs+Aq  of  1.298  sp.  gr.  contains  48%.    (Davy.) 
HNOs+Aq  of  1.298  sp.  gr.  contains  32-33%.     (Ber- 

thollet.) 

For  Ure's  table  of  sp.  gr.  of  HNO3+Aq,  see 
Watt's  Diet..  1st  ed. 

Sp.  gr.  of  HNO3+Aq  at  0°  and  15°. 


% 

HN03 

&   . 

Sp.  gr. 
at  0° 

Sp.  gr. 
at  15° 

100.00 

85.71 

1.559 

1.530 

99.84 

85.57 

1.559 

1.530 

99.72 

85.47 

1.558 

1.530 

99.52 

85.30 

1.557 

1.529 

97.89 

83.90 

1.551 

1.523 

97.00 

83.14 

1.548 

1.520 

96.00 

82.28 

1.544 

1.516 

95.27 

81.66 

.542 

1.514 

94.00 

80.57 

.537 

1.509 

93.01 

79.72 

.533 

1.506 

92.00 

78.85 

.529 

1.503 

91.00 

78.00 

.526 

1.499 

90.00 

77.15 

.522 

1.495 

89.56 

76.77 

.521 

1.494 

88.00 

75.43 

1.514 

1.488 

87.45 

74.95 

1.513 

1.486 

86.17 

73.86 

1.507 

1.482 

85.00 

72.86 

1.503 

1.478 

84.00 

72.00 

1.499 

.474 

83.00 

71.14 

1.495 

.470 

82.00 

70.28 

1.492 

.467 

80.96 

69.39 

1.488 

.463 

80.00 

68.77 

1.484 

.460 

79.00 

67.71 

1.481 

.456 

77.66 

66.56 

1.476 

.451 

76.00 

65.14 

1.469 

.445 

75.00 

64.28 

1.465 

.442 

74.01 

63.44 

1.462 

.438 

NITRIC  ACID 


543 


Sp.  gr.  of  HNO3,  etc.  —  Continued. 

Sp.  gr.  of  HNO3+Aq  at  15°.    a  =  %;b  =  sp. 

nloa 

NTb5 

Sp.  gr. 
at  0° 

Sp.  gr. 
at  15° 

gr.  if  %  is  N2O5;  c-sp.  gr.  if  %  is  HNO3. 

a 

b 

C 

a 

b 

c 

73.00 
72.39 
71.24 
69.96 
69.20 
68.00 
67.00 
66.00 
65.07 
64.00 
63.59 
62.00 
61.21 
60.00 
59.59 
58.88 
58.00 
57.00 
56.10 
55.00 
54.00 
53.81 
53.00 
52.33 
50.99 
49.97 
49.00 
48.00 
47.18 
46.64 
45.00 

62.57 
62.05 
61.06 
60.00 
59.31 
58.29 
.  57.43   . 
56.57 
55.77 
54.84 
54.50 
53.14 
52.46 
51.43 
51.08 
50.47 
49.71 
48.86 
48.08 
47.14 
46.29 
46.12 
45.40 
44.85 
43.70 
42.83 
42.00 
41.14 
40.44 
39.97 
38.57 

1.457 
1.455 
1.450 
1.444 
1.441 
1.435 
,1.430 
1.425 
1.420 
1.415 
1  .  413 
1.404 
1.400 
1.393 
1.391 
1.387 
1.382 
1.376 
1.371 
1.365 
.359 
.358 
.353 
.349 
.341 
.334 
.328 
.321 
.315 
.312 
.300 

1.435 
1.432 
1.429 
1.423 
1.419 
.414 
.410 
.405 
.400 
.395 
.393 
.386 
.381 
.374 
1.372 
1.368 
1.363 
1.358 
1.353 
1.346 
1.341 
1.339 
1.335 
1.331 
1.323 
1.317 
.312 
.307 
.398 
.295 
.284 

1 

2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 

1.007 
1.014 
1.021 
1.027 
1.034 
1.040 
1.047 
1.053 
1.061 
1.069 
1.076 
1.083 
1.091 
1.098 
1.104 
1.112 
.120 
.126 
.134 
.141 
.149 
.156 
.165 
.172 
.180 
.187 
.195 
.202 
.211 
.218 
.225 

1.006 
1.012 
1.018 
1.024 
1.029 
1.035 
1.040 
1.045 
I'.OSl 
1.057 
1.064 
1.070 
1.077 
1.083 
.089 
.095 
.100 
.106 
.112 
.120 
.126 
.132 
.138 
.145 
.151 
.159 
.166 
.172 
1.179 
1.185 
1.192 

5t 
52 
53 

54 
55 
56 
57 
58 
59 
60 
61 
62 
63 
64 
65 
66 
67 
68 
69 
70 
71 
72 
73 
74 
75 
76 
77 
78 
79 
80 
81 

1.372 
1.378 
1.385 
1.390 
1.396 
1.401 
1.407 
1.413 
1.418 
1.423 
1.427 
1.432 
1.436 
1.440 
1.445 
1.449 
1.452 
1.457 
1.461 
1.466 
.470 
.474 
.478 
.482 
.486 
1.490 
1.494 
1.499 
1.503 
1.507 
1.511 

1.323 
1.329 
1.335 
1.341 
1.346 
1.356 
1.358 
1.363 
1.369 
1.374 
1.380 
1.386 
1.390 
1.395 
1.400 
1.405 
1.410 
1.414 
1.419 
1.422 
1.427 
1.430 
1.435 
1.439 
1.442 
1.445 
1.449 
1.452 
1.456 
1.460 
1.463 

43.53 

37.31 

.291 

.274 

32 

1  .  232 

1.198 

82 

1.515 

1.467 

42.00 

36.00 

.280 

.264 

33 

1.240 

1.204 

83 

1.519 

1.470 

41.00 

35.14 

.274 

.257 

34 

1.248 

1.210 

84 

1.523 

1.474 

40.00 
39.00 
37.95 

34.28 
33.43 
32.53 

.267 
1.260 
1.253 

.251 
.244 
.237 

35 
36 
37 

1.255 
1.264 
1.271 

1.218 
1.225 
1.230 

85 
86 

87 

1.527 
1.530 

1.478 
1.481 
1.484 

36.00 

30.86 

1.240 

1.225 

38 

1.280 

1.236 

88 

1.488 

35.00 

29.99 

1.234 

1.218 

39 

.286 

1.244 

89 

1.491 

33.86 

29.02 

1.226 

1.211 

40 

.295 

1.251 

90 

1.495 

32.00 

27.43 

1.214 

1.198 

41 

.304 

1.257 

91 

1.499 

31.00 

26.57 

1.207 

1.192 

42 

312 

1  264 

92 

1.503 

30.00 

25.71 

1.200 

1.185 

43 

.318 

1.270 

93 

1.506 

29.00 

24.85 

:1.194 

1.179 

44 

.325 

1.276 

94 

1.509 

28.00 

24.00 

1.187 

.172 

45 

1.332 

1.284 

95 

1.512 

27.00 

23.14 

1.180 

.166 

46 

1.340 

1.290 

96 

1.516 

25.71 

22.04 

.171 

.157 

47 

1.346 

1.298 

97 

1.520 

23.00 

19.71 

.153 

.138 

48 

1.352 

1.304 

98 

1.523 

20.00 

17.14 

.132 

.120 

49 

1.360 

1.312 

99 

1.526 

17.47 

14.97 

.115 

1.105 

50 

1.366 

1.316 

100 

1.530 

15.00 

12.85 

.099 

1.089 

13.00 

11.14 

1.085 

1.077 

(Kolb,  calculated  by  Gerlach,  Z.  anal.  8.  292. 

11.41 

7.72 

9.77 
6.62 

1.075 
1.050 

1.067 
1.045 

Sp.  gr.  of  HNO3+Aq  at  17.5°. 

4.00 

3.42 

1.026 

1.022 

2.00 

1.71 

1.013 

1.010 

N^>5 

Sp.  gr. 

Njfos 

Sp.  gr. 

Nabs 

* 

Sp.  gr. 

0.00 

o  on 

i    nru~i 

OQOQ 

\J  .  \J\J 

.  t/iy  t7 

1  o 

(Kolb,  A.  ch.  (4)  10.  140.) 

6 

1.'038 

10 

1.'068 

lo 
14 

1.'096 

7 

1.045 

11 

1.075 

15 

1.104 

8 

1.053 

12 

1.082 

16 

1.111 

541 


NITRIC  ACID 


Sp.  gr.  of  HNO3,  etc.—  Continued. 

Most  accurate  table. 

%N206 

So.  gr. 

%  N205 

Sp.  gr. 

%N2C>5 

Sp.  gr. 

Sp.  gr.  of  HNO3+Aq  at  15°;  H2O  at  4°  =  1. 

17 

18 

1.118 
1.125 

40 
41 

1.294 
1.301 

63 
64 

1.434 
1.438 

Sp.  gr. 

%  N205 

%  HN03 

Kg.  HNO3 
in  1  1. 

1Q 

1  .  132 

'4.9 

1      OAC 

(•C 

IAAf) 

I  t  7 

20 

l!l40 

TTA 

43 

±  .  OUo 

1.315 

DO 

66 

.  i±f±£i 

1.447 

.000 

0.08 

0.10 

0.001 

21 

1.147 

44 

1.323   ! 

67 

1.451 

.005 

0.85 

1.00 

0.010 

22 

1.115 

45 

1.330 

68 

1.456 

.010 

1.62 

1.90 

0.019 

23 

1.163 

46 

1  .  338 

69 

1.460 

.015 

2.39 

2.80 

0.028 

24 

1.170 

47 

1.345 

70 

1.465 

.020 

3.17 

3.70 

0.038 

25 

1.178 

48 

1.352 

71 

1.469 

.025 

3.94 

4.60 

0.047 

26 

1.186 

49    • 

1.35$ 

72 

1.472 

.030 

4.71 

5.50 

0.057 

27 

1.194 

50 

1.364 

73 

1.476 

.035 

5.47 

6.38 

0.066 

28 

1.201 

51 

1.371 

74 

1.480 

.040 

6.22 

7.26 

0.075 

29 

1.209 

52 

1.377 

75 

1.484 

.045 

6.97 

8.13 

0.085 

30 

1.217 

53 

1.383 

76 

1.488 

.050 

7.71 

8.99 

0.094 

31 

1.221 

54 

1.389 

77 

1.492 

.055 

8.43 

9.84 

0.104 

32 

1.232 

55 

1.394 

78 

1.496 

.060 

9.15 

10.68 

0.113 

33 

1.239 

56 

1.400 

79 

1.500 

.065 

9.87 

11.51 

0.123 

34 

1.247 

57 

1.406 

80 

1.504 

.070 

10.57 

12.33 

0.132 

35 

1.255 

58 

1.412 

81 

1.508 

.075 

11.27 

13.15 

0.141 

36 

1.263 

59 

1.416 

82 

1.512 

.080 

11.96 

13.95 

0.151 

37 

1.271 

60 

1.421 

83 

1.516 

1.085 

12.64 

14.74 

0.160 

38 

1.279 

61 

1.426 

84 

1.519 

1.090 

13.31 

15.53 

0.169 

39 

1.287 

62 

1.430 

85 

1.523 

1.095 

13.99 

16.32 

0.179 

1.100 

14  67 

17.11 

0  188 

(Hager,  Comm.  1883.) 

l!l05 

15^34 

17!  89 

0^198 

Sp.  gr.  HNO3+Aq  at  17.5°. 

1.110 

'  16.00 

18.67 

0.207 

%N2O5 

Sp.  gr. 

%  N2O6 

Sp.  gr. 

%  N206 

Sp.  gr. 

.115 
.120 

16.67 
17.34 

19.45 
20.23 

0.217 
0.227 

10 
15 
20 
30 

1.068 
1.104 
1.140 
1.217 

40 
50 
60 

1.293 
1.361 
1.417 

70 

80 

85 

1.465 
1.500 
1.5.14 

.125 
.130 
.135 
.140 

18.00 
18.66 
19.32 
19.98 

21.00 
21.77 
22.54 
23.31 

0.236 
0.246. 
0.256 
0.266 

'  * 

•  • 

.145 

20.64 

24.08 

0.276 

(Hager,  Adjumenta  varia,  Leipzig,  1876.) 

.150 

21.29 

24.84 

0.286 

Sp.  gr.  of  HNO3+Aq  at  15°. 

.555 
1    IfiO 

21.94 
99  fin 

25.60 

9fi   ^fi 

0.296 

Oqrvc 

%  HN03 

Sp.  gr. 

%  HN03 

Sp.  gr. 

-L  .  JLIJU 

1.165 

£6  .  DU 

23.25 

£\J  .  OO 

27.12 

.  oUO 

0.316 

1 

1.00581 

26 

1  .  15869 

1.170 

23.90 

27.88 

0.326 

2 

1.01136 

27 

1.16660 

1.175 

24.54 

28.63 

0.336 

3 

1.01713 

28 

1.17371 

1.180 

25.18 

29.38 

0.347 

4 

1.02286 

29 

1.18073 

1.185 

25.83 

30.13 

0.357 

5 

.02851 

30 

1  .  18830 

1.190 

26.47 

30.88 

0.367 

6 

.03439 

31 

1  .  19552 

1.195 

27.10 

31.62 

0.378 

7 

.04019 

32 

1.20276 

1.200 

27.74 

32.36 

0.388 

8 

.04592 

33 

.20635 

1.205 

28.56 

33.09 

0.399 

9 

.05234 

34 

.21300 

1.210 

28.99 

33.82 

0.409 

10 

.05746 

35 

.22013 

1.215 

29.61 

34.55 

0.420 

11 

.06330 

36 

.22675 

1.220 

30.24 

35.28 

0.430 

12 

.  06951 

37 

.23347 

1.225 

30.88 

36.03 

0.441 

13 

.07581 

.      38 

.23980 

1.230 

31.53 

36.78 

0.452 

14 

.08126 

39 

.24510 

1.235 

32.17 

37.53 

0.463 

15 

.08843 

40 

.25235 

1.240 

32.82 

38.29 

0.475 

16 

.09500 

41 

.25850 

1.245 

33.47 

39.05 

0.486 

17 

1  .  10102 

42 

.26475 

1.250 

34.13 

39.82 

0.498 

18 

1.10725 

43 

.27125 

1.255 

34.78 

40.58 

0.509 

'  19 

1.11321 

44 

.28895 

1.260 

35.44 

41.34 

0.521 

20 

1.12024 

45 

.28450 

1.265 

36.09 

42.10 

0.533 

21 

1.12714 

46 

.29110 

1.270 

36.75 

42.87 

0.544 

22 

1  .  13349 

47 

.29780 

1.275 

37.41 

43.64 

0.556 

23 

1  .  13890 

48 

.30443 

1.280 

38.07 

44.41 

0.568 

24 

1  .  14460 

49 

.31101 

1.285 

38.73 

45.18 

0.581 

25 

1.15164 

50 

.31722 

1.290 

39.39 

45.95 

0.593 

1.295 

40.05 

46.72 

0.605 

(Squires,  Pharm.  Era,  Jan.  1891.) 

NITRATES 


545 


Sp.  gr.  of  HNO3,  etc.  —  Continued. 

Sp.  gr. 

of  N-HNO3+Aq  at  18°/4°  =  1.0324. 

W4                     1  OA^       /*f\       f  ff\    \ 

ifr,    wvm. 

(Loomis, 

.  Ann.  18i: 

>o,  ou.  oou.; 

Sp.  gr. 

%  N205 

%  HN03 

in  11. 

Sp.  gr.  (reduced  to  a  vacuum)  of  HNO3  from 
78-100%       concentration       at      4°/4°, 
14.20/4°and24.2°/40. 

1.300 
1  .  305 

40.71 
41.37 

47.49 
48.26 

0.617 
0.630 

1  310 

42  06 

49.07 

0.643 

1.315 

Ioon 

42'  76 

49^89 

CA     *71 

0^656 

O/J/JA 

frf    TTTVT/^ 

Sp.  gr. 

.620 
1.325 

44!  17 

oU.  /I 
51.53 

.659 
0.683 

%  MJNUs 

4°/4° 

14.2°/4° 

24.2°/4° 

1.330 
1.335 
.340 

44.89 
45.62 
46.35 

52.37 
53.22 
54.07 

0.697 
0.710 
0.725 

78.22 
79.14 

1.47129 

1.45504 
1.46011 

1.43964 
1.44372 

.345 
.350 

48.07 
47.82 

54.93 
55.79 

0.739 
0.753 

79.59 
81.97 

1  .  47496 
1.48391 

1.46680 

1^45092 

.355 

48.57 

56.66 

0.768 

84.90 

1  .  49495 

.360 
.365 

49.35 
50.13 

57.57 

58.48 

0.783 
0.798 

85.21 

85.80 

1.49581 

i'.  47826 

I.  46224 

.370 

50.91 

59.39 

0.814 

87.55 

i.502li 

0*7  er 

er  i     &f\ 

f*f\    on 

Ooork 

87.90 

.48491 

1  .  46891 

.375 

oor\ 

51.69 

ero    co 

60.30 

/j  -|       O*T 

.829 

OO  A  C 

89.73 

1  50898 

49125 

.  .  o8() 
.385 
.390 
.395 
.400 

52.52 
53.35 
54.20 
55.07 
55.97 

bl.27 
62.24 
63.23 
64.25 
65.30 

.846 
0.862 
0.879 
0.896 
0.914 

92.34 
94.04 
95.62 
96.64 

1.51804  ' 
1.51949 
1  .  52192 
1.52510 

.49968 
.50149 
.50358 
.50632 

1.48264 
1.48516 
1.48677 

1.48887 

1.405 
1.410 
1.415 

56.92 

57.86 
58.83 

66.40 
67.50 
68.63 

0.933 
0.952 
0.971 

97.33 

98.07 
99.97 

i.532i2 
1.54212 

.50911 
.51298 
.52236 

1.49137 
1.49543 
1.50394 

1.420 
1.425 

59.83 
60.84 

69.80 
70.98- 

0.991 
1.011 

(Veley  and  Manley,  Chem.  Soc. 

1  f\~t  £*    \ 

1903,  83. 

1.430 

61.86 

72.17 

1.032 

1016.) 

1.435 
1.440 

62.91 
64.01 

73.39 

74.68     • 

1.053 
1.075 

Sp.  gr.  at  20°  of  HNO3+Aq  containing  M 
g.  mols.  HNO3  per  liter. 

1.445 

65.13 

75.98 

.098 

M          0.025        0.05 

0.075 

0.10 

.450 

66.24 

77.28 

.121 

Sp.  gr.  1. 

000926  1.001798  1.002653  1.003496 

.455 

67.38 

78.60 

.144 

.460 

68.56 

79.98 

.168 

M          0.25          0.5 

0.75 

1.0 

.465 

69.79 

81.42 

.193 

Sp.gr.  1. 

008481  1.01686     1.02503     1.0336 

.470 

71.06 

82.90 

.219 

M          2.0 

.475 

72.39 

84.45 

.246 

Sp.  gr.  1.0670 

.480 

.485 

73.76 
75.18 

86.05 
87.70 

.274 
.302 

(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38.  732.) 

1.490  . 
1.495 

76.80 

78.57 

89.60 
91.60 

.335 
.369 

For  sp 
H2SO4. 

.  gr.  of  HN03+H2S04, 

see  under 

1.500 

80.65 

94.09 

.411 

Partition    coefficient   for   HNO3   between 

1.501 

81.09 

94.60 

.420 

ether  and  H2O  is  increased  by  the  addition 

1.502 

81.50 

95.08 

.428 

of  nitrates.    (Tanret, 

C.  R.  1897.  124.  464.1 

1.503 
1.504 
1.505 
1.506 

81.91 
82.29 
82.63 
82.94 

95.55 
96.00 
96.39 
96.76 

.436 
.444 
.451 
.457 

The  hydrates  described  by  Erdmann  do 
not  exist.    There  are  only  two  authentic  hy- 
drates,   the    mono-    and    the    tri-hydrate. 
(Kiister,  Ch.  Z.  1904,  28.  132.) 

1.507 
1.508 
1.509 
1.510 
1.511 
1.512 

83.26 
83.58 
83.87 
84.09 
84.28 
84.46 

97.13 
97.50 
97.84 
98.10 
98.32 
98.53 

.464 
.470 
.476 
.481 
.486 
.490 

The  composition  of  the  hydrates  formed 
by  HNO3  at  different  dilutions  is  calculated 
from  determinations  of  the  lowering  of  the 
fr.-pt.  produced  by  HNO3  and  of  the  con- 
ductivity and  sp.  gr.  of  HNO3+Aq.    (Jones, 
Am.  Ch.  .1.  1905.  34.  328.1 

1.513 

84.63 

98.73 

.494 

1.514 

84.87 

98.90 

.497 

£)mitric 

acid,  H2N40U  =  2N206, 

H20. 

1.515 
1.516 
1.517 

84.92 
85.04 
85.15 

99.07 
99.21 
99.34 

.501 
.504 

;507 

;    Fumes 
evolution 

6Q4.0  ^ 

on  air.     Miscible  with 
of  much  heat.    (Weber 

H2O,  with 
,  J.  pr.  (2) 

1.518 

85.26 

99.46   . 

.510 

•    '  >  I  _  . 

1.519 

85.35 

99.57   , 

.512 

Nitrates. 

1.520 

85.44 

99  .  67 

.515 

All  nitrates  are  sol.  in  H2O  except  a  few 

(Lunge  and  Rey,  Z.  f  .  angew.  Ch.  1891.  165.) 

basic  compounds.    Most  nitrates  are  insol.  in 

546 


NITRATE,  ALUMINUM,  BASIC 


cone.  HNOs+Aq;  many  are  sol.  in  alcohol; 

100  pts.  H2O  dissolve  183  pts.  NH4NO3  at 

some  are  sol.  in  glycerine. 

19.5°.    (Mulder.) 

Aluminum    nitrate,   basic,  2A12O3,   3N2O6+ 
3H2O. 

Solubility  in 

H2O  at  t°. 

Sol.  in  H2O.    (Ordway,  Sill.  Am.  J.  (2)  26. 

OAO   "\ 

t° 

Specific  gravity 
of  the  saturated 

Mols.  of  NH4N03 
soluble  in  100 

zOo.) 
Basic  aluminum  nitrates  containing  2  mols. 

solution 

mols.  of  water 

or  less  of  A12O3  to  one  of  N2O5  may  be  ob- 

12.2 

1  .  2945 

34.50 

tained  sol.  in  H2O,  but  the  compounds  con- 

20^2 

1.3116 

43.30 

taining  more  than  2  mols.  A1203  are  insol.  in 

23.0 

.3159 

46.57 

H2O.    (Ordway,  I.  c.) 
2A12O3,  N2O6+10H2O.    (Ditte,  C.  R.  110. 

25.0 

27.7 

.3197 
.3257 

48.19 
51.67 

782.) 

28  0 

3260 

51.86 

Al6O14Hio,  HNO3.    Sol.  in  H2O.    (Schlum- 
berger,  Bull.  Soc.  1895,  (3)  13.  59.) 

3o!o 

30.2 

!3299 
.3308 

54^40 
54.61 

Aluminum  nitrate,  A1(NO3)3+9H2O. 
Deliquescent.    Very  sol.  in  H2O,  HNO3+ 
Aq,  or  alcohol.    (Berzelius.) 
Melts  in  its  crystal  H2O  at  72.7°.    (Ordway. 
Sol.  in  1  pt.  strong  alcohol.    (Wenzel.) 
Difficultly  sol.  in  acetone.     (Naumann,  B. 

31.9 
32.1 
32.7 
34.0 
35.0 
35.1 
35.6 

.3348 
.3344 
.3356 
.3375 
.3394 
.3397 
.3408 

57.20 
57.60 
57.90 
58.89 
59.80 
60.00 
60.62 

1904,  37.  4328.) 
Insol.   in   ethyl   acetate.      (Naumann,    B. 

36.0 
36  6 

.3412 
3420 

61.00 

1910,  43.  ai4.) 

37'5 

]3432 

62^90 

Ammonium  nitrate,  NH4NO3. 

38.0 

.3438 

63.60 

Deliquescent. 

Sol.  in  0.502  pt.  H2O  at  18°.     (Karsten.) 
Sol.  in  0.54  pt.  H2O  at  10°.     (Harris,  C.  R.  24.  816.) 

38.5 
39.0 
39.5 

.3440 
.3448 
.3460 

64.10 
65.09 

65.88 

Much  more  sol.  is  hot  than  cold  H2O.     (Harris.) 

40.0 

1.3464 

66.80 

Sol.  in  2  pts.  H2O  at  15.5°  and  0.5  pt.  boiling  H2O. 

(Fourcroy.) 
Sol.  in  1  pt.  cold,  and  0.5  pt.  boiling  H2O.   (Fourcroy.) 

(Miiller 

and-Kaufmann,  Z.  phys.  Ch.  1903 

Sol.  in  0.5  pt.  H2O  at  18°.     (Berzelius.) 

42.  4 

yy.; 

Sol.  in  2  pts.  H2O  at  18°.     (Abl.) 

Decomp.  by  boiling  H2O. 

Solubility  in 

H20  at  t°. 

Solubility  in  100  pts.  H2O  at  t°. 

G.  NH4NO3 

t° 

Pts. 

t° 

Pts. 

0 

Pts. 

t° 

per  100  g. 

Solid  phase 

t 

NH4NO3 

t 

NH4NO3 

NH4NO3 

solution 

water 

0 
1 

97 
101 

24 
25 

205 
210 

48 
49 

351 
358 

0 
12.2 

54.19 
60.53 

118.3 
153.4 

NH4N03,  rhomb.  0 

2 

105 

26 

216 

50 

365 

20  2 

65  80 

192  4 

,, 

3 
4 
5 
6 

109 
113 
117 
121 

27 
28 
.29 
30 

221 
226 
232 
238 

51 
52 
53 
54 

372 
379 
387 
395 

25.Q 
30.0 
32.1 

68^17 
70.73 
71.97 

2U.2 
241.8 
256.9 

NH4N03,  rhomb.  £  + 
rhomb,  ft 

7 
8 

125 
130 

31 
32 

244 
250 

55 
56 

402 
410 

35 
40 

72.64 
74  82 

265.8 
297.0 

NH4NO3,  rhomb,  a 

9 

134 

33 

256 

57 

418 

50 

4  rr  .  O^w 

77.49 

344.0 

M 

10 

139 

34 

262 

58 

425 

60 

80^81 

421  io 

(l 

11 

143 

35 

268 

59 

433 

70 

S3.  32 

499  'o 

(J 

12 

148 

36 

274 

60 

441 

80 

85  25 

580  o 

„ 

13 
14 

152 
157 

37 

38 

280 

286 

61 
62 

449 
457 

90 
100 

88^08 

QQ    71 

740  '.0 
871.0 

NH4NOs,  rhomb.    (?) 

15 

161 

39 

292 

63 

465 

i\J\J 

Ot/  .  f  1 

16 

166 

40 

298 

64 

473 

(SeidelPs  Solubilities  1st  ed.  28.    Calc.  from 

17 

170 

41 

304 

65 

481 

Miiller  &   Kauffmann,   see  above,   and 

18 

175 

42 

311 

66 

490 

Schwarz.  Ostwald's  Lehrb.,  p.  425.) 

19 

180 

43 

317 

67 

499 

20 

185 

44 

324 

68 

508 

100  g 

NH4NO3+Aq  contain: 

21 

190 

45 

331 

69 

517 

54.19  g.  NH4NO 

3at    0°. 

22 

195 

46 

337 

70 

526 

70  10  g         " 

"  30°. 

23 

200 

47 

344 

84.03  g. 

"  70°. 

(Mulder,  Scheik.  Verhandel.  1864.  95.) 

(de  Waal,  Dissert.  Leiden,  1910.) 

NITRATE,  AMMONIUM 


547 


70.19  g.  NH4NO3  are  contained  in  100  g. 

Sp.  gr.  of  NH4NO3+Aq. 

NH4NO3+Aq  sat.  at  30°.     (Schreinemakers 

and  de  Baat,  Arch.  neer.  Sc.   1911,  (2)  16. 

%  NH4NO3' 

Sp.  gr.  16°/  16° 

415.) 
60  pts.  NH4NO3  mixed  with  100  pts.  H2O 
lower  the  temperature  from  13.6°  to  —13.6°, 
that  is  27.2°,  but  if  the  initial  temperature  is 
0°  it  will  fall  only  to  —  16.7°,  the  freezing- 
point  of  the  mixture.     (Rudorff,  B.  2.  68.) 

0 
0.6419 
1.4101 
2.7501 
5.4890 
11.7981 

.000000 
.000271 
.000593 
.001153 
.002300 
.004916 

Sp.  gr.  of  NH4NO3+Aq  at  18°. 

23.4480 
47  9500 

.009758 
019952 

Pts.  NH4NO3             Pts.  H2O                    Sp.  gr. 

(Dijken.  Z.  phys.  Ch.  1897,  24.  107.) 

80                     1800                 1  .  0180 

80                      900                 1.0331 

Sp.  gr.  20°/4°  of  a  normal  solution  of  NH4NO3 

80                      360                 1.0743 

=  1.030435;  of  a  0.5-normal  solution  1  =  .014505. 

(Haigh,  J.  Am.  Chem.  Soc.  1912,  34.  1151.) 

(Thomsen  and  Gerlach,  Z.  anal.  28.  520.) 
Sp.  gr.  of  NH4NO3+Aq  at  15°. 

B.-pt.     of    NH4NO3-fAq    containing    pts. 
NH4NO3  to  100  pts.  H2O.    G  =  according 
to  Gerlach  (Z.  anal.  26.  445);  L=  accord- 

% NH4NO3 

Sp.  gr. 

%  NH4NO3 

Sp.  gr. 

ing  to  Legrand  (A.  ch.  (2)  59.  426.) 

5 

1.0201 

30 

1.1304 

* 

^ 

10 

1.0419 

40 

1.1780 

G 

L 

i 

G 

L 

20 

1.0860 

50 

1.2279 

pq 

ffl 

(Kohlrausch,  W.  Ann.  1879.  1.) 

101° 
102 

10 
20 

10 

20.5 

140° 
141 

682 
719 

770.5 

Sp.  gr.  of  NH4NO3+Aq  at  17.5°. 

103 

30 

31.3 

142 

737 

840  '  6 

104 

41 

42  4 

143 

765 

%  NH4N03 

Sp.  gr. 

%  NH4N03 

Sp.  gr. 

105 

1  f\G 

52 

fiO 

53.8 

144 

1  A  K. 

793 

915.5 

1 

1.0042 

33 

1  .  1454 

106 
107 

OO 

74 

77^3 

145 
146 

853 

995.5 

2 

1.0085 

34 

1.1502 

108 

85 

89.4 

147 

883 

3 

.0127 

35 

1  .  1550 

109 

96 

101.9 

148 

914 

1081.5 

4 

.0170 

36 

1.1598 

110 

108 

114.9 

149 

945 

5 

.0212 

37 

1  .  1646 

111 

120 

128.4 

150 

977 

U73.5 

6 

.0255 

38 

.1694 

112 

132 

142  4 

551 

1009 

7 

.0297 

39 

.1742 

113 

145 

156.9 

152 

1043 

1273 

8 

1.0340 

40 

.1790 

114 

158 

172 

153 

1079 

9 

1.0382 

41 

.1841 

115 

172 

188 

154 

1116 

1383 

10 

1.0425 

42 

.1892 

116 

187 

204.4 

155 

1155 

11 

1.0468 

43 

.1942 

117 

202 

221.4 

156 

1196 

1504" 

12 

1.0512 

44 

.1994 

118 

217 

238  4 

157 

1238 

13 

1.0555 

45 

.2045 

119 

232 

256.8 

158 

1281 

1637 

14 

1.0599 

46 

.2096 

120 

248 

275.3 

159 

1325 

15 

1.0642 

47 

.2147 

121 

265 

160 

1370 

1775 

16 

1.0686 

48 

.2198 

122 

283 

3l4 

161 

1417 

17 

1.0729 

49 

.2249 

123 

301 

162 

1464 

1923' 

18 

1.0773 

50 

.2300 

124 

319 

354 

163 

1511 

19 

1.0816 

51 

.2353 

125 

337 

164 

1558 

2084' 

20 

1.0860 

52 

.2407 

126 

356 

396 

165 

1606 

21 

1.0905 

53 

.2460 

127 

376 

166 

1653 

22 

.0950 

54 

.2514 

128 

396 

440.2 

167 

1700 

23 

.0995 

55 

1.2567 

129 

417 

168 

1748 

24 

.1040 

56 

1.2621 

130 

439 

487.4 

169 

1796 

25 

.1085 

57 

1.2674 

131 

461 

170 

1844 

26 

.1130 

58 

.2728 

132 

484 

537.3 

180 

2400 

oo 

27 

.1175 

59 

.2781 

133 

507 

190 

3112 

28 

1  .  1220 

60 

.2835 

134 

530 

590 

200 

4099 

29 

1.1265 

61 

.2888 

135 

554 

210 

5618 

30 

1.1310 

62 

.2942 

136 

578 

645 

220 

8547 

31 

1.1358 

63 

.3005 

137 

603 

230 

16950 

32 

1.1406 

64 

.3059 

138 

629 

ere 

705.5 

240 

00 

... 

(Gerlach,  Z.  anal.  27.  310.) 

139 

DOO 

*   •   * 

•  •  • 

*    "    * 

548 


NITRATE,  AMMONIUM 


Ch 


Very  sol.  in  HNO3+Aq.      (Schulz,  Zeit. 
.  1869.  531.) 


Solubility  of  NH4NO3  in  HNO3. 


Solution 
temp. 

%  by  wt. 
NH4N03 

Solid  phase 

+8° 

21.1 

NH4NO3,  2HNO3  (solu- 

tion in  HNO3) 

23.0 

28.7 

tt 

28.5 

34.5 

11 

29.5* 

38.8 

(solution  in  NH4NO3) 

27.5 

44.6 

u 

27.0 

45.8 

t( 

23.5 

49.4 

(( 

23.0 

50.0 

u 

17.5 

54.0 

(( 

16.5 

54.3 

(I 

4.0 

45.8 

NH4NO3,  HNO3  labile 

(solution  in  HNO3) 

9.5 

49.4 

(i 

11.0 

51.7 

u 

11.5 

52.7 

u 

12.0 

54.3 

u 

12.0 

54.7 

(I 

11.5 

57.6 

(solution  in  NH4NO3) 

11.5 

54.0 

NH4N03  (labile) 

14.5 

54.3 

a 

17.0 

54.7 

stable 

26.0 

55.9 

n 

27.0 

56.2 

(( 

33.5 

57.5 

It 

49.0 

60.4 

u 

79.0 

68.1 

fl 

*  Mpt.  of  NH4NO3,  2HNO3. 

(Groschuff.  Z.  anorg.  1904,  40.  6.) 

Solubility  of  NH4NO3  in  NH4OH+Aq. 


Grams  of 
NH4N03 

Grams  of 
NH3 

Molecules 
ofNBUNOs 
in  100 
molecules 
NH4N03  + 
NH3 

Temperature  at 
which  the  solu- 
tions are  in 
equilibrium  with 
the  solid  phase 

100. 

about  168° 

6^7578 

61  0588 

74.2 

109.8 

0.6439 

0.0665 

67.3 

94.0 

4.2615 

0.7747 

53.8 

68.8 

0.7746 

0.1857 

47.0 

35.9 

0.9358 

0.2352 

45.9 

33.3 

0.7600 

0.2607 

38.3 

0 

0.9675 

0.3515 

36.9 

—  10.5 

0.8308 

0.3700 

32.3 

-30.0       • 

0.9526 

1.2457 

13.9 

-44.5 

1.3918 

4.4327 

6.25 

—  60 

0 

100 

0 

about  —80 

(Kuriloff,  Z.  phys.  Ch.  1898,  26.  109.) 

NH4NO3+NH4C1. 

100  pts.  H2O  dissolve  29.1  pts.  NH4C1  and 
173.8  pts.  NH4NO3.  (Rudorff,  B.  6.  484.) 

Sol.  in  sat.  NH4Cl+Aq  with  pptn.  of 
NH<C1  until  a  state  of  equilibrium  is  reached. 
(Karsten.) 


Addition  of  KC1O3  to  NH4Cl+Aq  prevents 
pptn.  of  NH4C1,  and  dissolves  any  NH4C] 
that  may  have  been  pptd.  (Margueritte,  C. 
R.  38.  306.) 

See  also  under  Ammonium  chloride. 

NH4NO3+KNO3. 

100  pts.  H2O  dissolve: 


At  9° 

At  11° 

At  15° 

(1)         (2) 

(3)        (4) 

(5)        (6) 

KNO3... 

20.2 

40.6 

26.0 

46.2 

NH4NO3 

88.8 

143 

130.4 

161 

2,  Sat.  at  11°  with  NH4NO3  and  then  at  9° 
with  KNO3;  5,  sat.  at  11°  with  NH4NO3  and 
then  at  15°  with  KNO3.  (Mulder.) 

Sol.  in  sat.  HNO3+Aq  without  causing  ppt. 
(Karsten)  ;  with  separation  of  KNO3  (RudorrT) 

Composition  of  solution  is  dependent  on  the 
relative  excess  of  the  salts  present.  (  Riidorff.) 

100  pts.  H2O  dissolve  77.1  pts.  NaNO3  and 
162.9  pts.  NH4NO3  at  16°.  (Rudorff,  B.  6. 
484.) 

If  a  sat.  solution  of  NH4NO3+Aq  at  11°  is 
sat.  with  Ba(NO3)2  at  9°,  100  pts.  H2O 
dissolve: 


NH4NO3.... 

Ba(N03)2... 

At  11° 

101.3 
6.2 

At  9° 

143 

els 

(Mulder.) 
Solubility  of  NH4NO3+AgNO3  in  H2O  at  t 


t° 

AgNOs 

NH4NO3 

Solid  phase 

—  7.3° 
—10.7 
—14.9 

—14.8 
—18.7 

—17.4 

47.1 
44.52 
42.0 

39.51 
15.99 

0 

0 
8.43 
16.80 

18.79 
37.30 

41.2 

Ice+AgNOs,  rhomb. 

Ice+AgNOs,  NH4NOs 
+AgNOs  rb. 
Ice+AgNOs,  NH4N03 
Ice+AgNOs,  NH4NOs 
+NH4NOs  0.  rb. 
Ice+NH4N03,  #.rb. 

0 

18 
30 
S    55 
109.6 

50.36 

55.36 
58.89 
63.32 
67.9 

19.59 

22.06 
23.42 
26.12 
32.1 

AgNOs,  NH4N03  + 
AgNOs,  rb. 

0 

18 
30 
40 

55 
101.5 

22.13 

27.07 
29.76 
32.68. 

36.60 
47.5 

44.87 

49.22 
52.50 
52.22 

52.38 
52.5 

AgNOs,  NH4N03  + 
NH4NOs  0.  rb. 

AgNOs,  NH4NOs  + 
NH4NO3  a  rb. 

AgNOs,  NH4NO3  + 
NH4NOs,  rbd. 

1911  (2)  15.  414.) 


Baat,  Arch.  neer.  Sc. 


NITRATE,  AMMONIUM 


549 


Solubility  in  NH4NO3  and  AgNO3  in  H2O 

Solubility  of  NH4NO3+(NH4)2SO4  in  H2O 

at  30°. 

at  30°. 

Composition  of  the 
solution 

NH4NO3 

(NH4)2So4                      Solid  phase 

Solid  phase 

NH4N03 

AgNOs 

70.1 
67.63 

0                            NH4NO3 
2.38 

0 

6.59 
15.62 
23.40 
23.45 
24.33 
26.22 
28.86 
34.47 
39.60 
45.44 

73.0 
69.08 
63.27 
58.84 
58.93 
57.93 
55.32 
52.45 
45.85 
41.09 
35.62 

AgNOs 
u 

it 
AgNOs  +  AgNOs,  NH4N03 

AgNOs,  NH4NO3 
0 

66.93 

63.84 
58.06 

52.75 
49.80 

37.20 
19.91 
12.05 

3.46      NH4NO3+(NH4)2SO4, 
3NH4NO3 

4  .  96           (NH4)  2SO4,  3NH4NO3 
8  .  22      (NH4)2S04,  3NH4N03  + 
(NH4)2SO,  2NH4NO3 
11  .42             (NH4)2SO4,  2NH4NO3 
13.27      (NH4)2SO4,  2NH4NO3  + 
(NH4)2S04 
19.48                     (NH4)2SO4 
28.83 
34.7 

52.49 

29.77 

NH4N03+AgN03,  NH4N03 

44  .  1 

52.11 

52.89 

29.86 
29.66 

t 
i 

(Schreinemakers  and  Haenen,  Chem.  Weekbl. 
1909,  6.  51.) 

54.12 

27.75 

NH4NO?, 

58.64 

21.31 

u 

63.59 
70.10 

12.51 
0 

„   .      u 

Solubility  of  NH4N03+(NH4)^S04  in  H2O. 

Temp.  =0° 

(Schreinemakers  and  de  Baat,  Z.  phys.  Ch. 

lyuy,  DO.  o/z.; 

• 

O 

5 

Solubility  of  NH4NO3+NaNO3  in  H2O  at  t°. 

1 

s 

Solid  phase 

g.  per  100  g.  H2O 

Y 

t° 

Sp.  gr. 

0 
5.61 

41.4 
37.89 

(NH4)2SO4 

NH4N03                NaNOs 

0 

0                  73.33 
105.5               66 
118.4                 0 

1.354 
1.407 
1.264 

29.58 
29.81 
31.04 

41.64 
21.33 
20.40 

(NH4)2SO4-HNH4)2S04,  2NH4NO» 
(NH4)3S04>  2NH4N03 

30.87 

20.43 

(NH4)  2SO4,  2NH4NO3  +(NH4)  2SO4, 

15 

0                   83.9 
24.03             81.21 
42.81             79.34 
64.6               78.06 

1.375 
1.386 
1.392 
1.401 

31.61 
45.99 
49.12 

19.50 
9.53 
6.00 

3NH4N03 
(NH4)2SO4,  3NH4NO3 
(NH4)2SO4,  3NH4NO3+NH4NO» 
NH4NO3 

110.9               75.81 

1.417 

54.19 

0 

152.                 75.35 

1.428 

155.3               75.38 

1.429 

Temp.  =70° 

156.1               60.76 

1.405 

159                  36.50 

1.364      . 

d 

d 

160                  27.79 

1.350 

KO^S 

Solid  phas6 

162.3               17.63 

1.330 

H 

M 

167.4                 0 

1.298 

* 

g 

30 

0                   96.12 

1.401 

0 

47.81 

(NH4)2SO4 

220.8               88.31 

1.450 

11.10 

40.81 

14 

232.6                 0 

1.329 

70.15 

6.71 

(NH4)2SO4  +  (NH4)»SO4,  2NH4NO3 

71  .58 

5.82 

(NH4)2SO4,  2NH4NO3 

(Fedotieff  and  Koltunoff,  Z.  anorg.  1914,  85. 

73.48 

5^14 

(NH4)2S04,  2NH4NOs+(NH4)2SO4, 

251.) 

3NH4NOs 

76.01 

3.96 

(NH4)2S04,  3NH4NO3 

80.25 

2.68 

" 

81.01 

2.45 

(NH4)2SO4,  3NH4N03+NH4N03 

81.38 

2.41 

NH4N03 

84.03 

0 

it 

(de  Waal.   Dissert.   Leiden.   1910.) 

550 


NITRATE,  AMMONIUM  HYDROGEN 


Very  easily  sol.  in  liquid  NH< 
Am.  Ch.  J.  1898,  20.  826.) 


(Franklin, 


1  pt.  NH4NO3  dissolves  in  2.29  pts.  alcohol  of  66.8% 
at  25°.  (Pohl,  W.  A.  B.  6.  599.) 

1  pt.  NH4NO3  dissolves  in  1.1  pt.  boiling  alcohol. 

100  pts.  absolute  methyl  alcohol  dissolve 
17.1  pts.  at  20.5°.  (de  Bruyn,  Z.  phys.  Ch. 
10.  783.) 

100  g.  absolute  methyl  alcohol  dissolve 
14.6  g.  NH4NO3  at  14°  and  16.3  g.  at  18.5°. 
(Schiff  and  Monsacchi,  Z.  phys.  Ch.  1896,  21. 
277.) 

100  pts.  absolute  ethyl  alcohol  dissolve  3.8 
pts.  at  20.5°:  (de  Bruyn,  Z.  phys.  Ch.  10. 
783.) 

100  g.  absolute  ethyl  alcohol  dissolve  4.6  g. 
at  14°.  (Schiff  and  Monsacchi,  Z.  phys.  Ch. 
1896,  21.  277.) 

Solubility  of  NH4NO3  in  H2O  is  decreased 
by  presence  of  ethyl  alcohol  but  increased  by 
presence  of  methyl  alcohol.  NH4NO3  is  only 
very  si.  sol.  in  abs.  ethyl  alcohol  and  the  sol- 
ubility increases  slowly  with  rise  in  temp.;  it  is 
more  sol.  in  abs.  methyl  alcohol  and  the 
solubility  increases  rapidly  with  rise  in  temp. 
(Fleckenstein,  Phys.  Zeit.  1905,  6.  419.) 


Solubility  in  methyl  alcohol +Aq.  at  30°. 


%  by  wt.  H2O 

%  by  wt. 
alcohol 

%  by  wt. 
NH4NO3 

29.9 
21.6 
20.6 
16.5 
11.5 
0 

0 
24.5 
31.3 
46.0 
59.4 
83.3 

70.1 

53.9 
48.1 
37.5 
29.1 
16.7 

(Schreinemakers,    Z.    phys.    Ch.    1909,    65. 
556.) 


Solubility  of  NH4NO3  in  ethyl  alcohol +Aq. 
at  30°.    Composition  of  sat.  solution. 


%  by  wt.  H2O 

%  by  wt.  alcohol 

%bywt.NH4NO3 

29.9 

0 

70.1 

26.9 

18.6 

54.5 

23.2 

39.3 

37.5 

18.3 

58.5 

23.2 

11.6 

76.5 

11.9 

5.8 

86.2 

8.0 

0 

96.4 

3.6 

(Schreinemakers,    Z. 

555.) 


Ch.    1909.    66. 


Solubility  of  NH4NO3  in  alcohol. 


t° 

%  NH4N03 

%  Alcohol 

%  H20 

0 

54.19 

0 

45.81 

42.69 

12.70 

44.61 

1.96 

97.93 

0.11 

<o 

70.10 

0 

29.90 

59.83 

10.60 

29.57 

8.06 

85.30 

6.64 

3.60 

96.51 

0 

70 

84.03 

0 

15.97 

72.37 

11.12 

16.51 

61.11 

22.87 

16.02 

41.25 

44.64 

14.11 

24.71 

67.23 

8.06 

7.51 

92.49 

0 

(de  Waal.  Dissert.  Leiden,  1910.) 


Sp.    gr.    of    alcoholic    solution    of    NH4NO3 
at  15°. 


Pts. 

NEUNOj 

Pts. 
alcohol 

Sp.  gr. 

0 
2 
4 
6 

100 
98 
96 
94 

0.83904 
0.84746 
0.85604 
0.86524 

(Gerlach,  Z.  anal.  28.  521.) 


(Naumann,  B.  1914, 
(Naumann,  B. 


Insol.  in  benzonitrile. 
47.  1370.) 

Insol.  in  methyl  acetate. 
1909,42.3790.) 

Very  si.  sol.  in  acetone.    (Krug  and  M'El- 
roy,  J.  Anal.  Ch.  6.  184.) 

Sol.  in  acetone.     (Eidmann,  C.  C.  1899, 
II.  1014.) 

Ammonium  hydrogen  nitrate,  NH4H(NO3)2. 
Sol.  in  H2O.    (Ditte,  C.  R.  89.  576,  641.) 
Decomp.  by  H2O.    (Groschuff,  B.  1904,  37. 

1487.) 

Ammonium  dihydrogen  nitrate. 

NH4H2(N03)3. 
Sol.  in  H2O.    (Ditte.) 

Solubility  in  H2O. 


Solution 
temp. 

%  by  wt. 
NH4NOs 

%  by  wt. 
HNO3 

—8.0 
—2.5 
+3.0 
3.5 
19.5 
25.0 
29.5mpt. 

34.2 
34.8 
35.4 
36.0 
37.4 
38.1 
38.8 

53.9 
54.8 
55.8 
56.8 
58.9 
60.0 
61.2 

(Groschuff,  Z.  anorg.  1904,  40.  7.) 


NITRATE,  AMMONIUM,  AMMONIA 


551 


Ammonium  cerous  nitrate,  3NH4NO3, 
2Ce(NO3)3  +  12H2O. 

Very  deliquescent.  Very  sol.  in  H2O  and 
alcohol.  (Holzmann,  J.  pr.  84.  78.) 

-HOH2O.  Hygroscopic.  Sol.  in  H2O. 
(Drossbach,  B.  1900,  33.  3507.) 

2NH4NO3,  Ce(NO3)3+4H2O.  As  above. 
(Marignac,  A.  ch.  (4)  30.  64.) 

Solubility  in  H2O. 
100  g.  H2O  dissolve  at: 
8.75°       25°  45° 

235.5  296.8        410.2  g.  anhydrous  salt, 

60°  65.06° 

681.2        817.4  g.  anhydrous  salt. 

(Wolff,  Z.  anorg.  1905,  45.  98.) 

Ammonium  eerie  nitrate,  2NH4NO3, 
Ce(N03)4. 

Very  sol.  in  H2O  without  decomp.  Sol.  in 
HNO3.  (Meyer,  B.  1900,  33.  2137.) 

Sol.  in  alcohol.  (Meyer,  Z.  anorg.  1901, 
27.  369.) 

Solubility  in  H2O. 
100  g.  H20  dissolve  at  t°: 
25°  35.2°         45.3° 

140.9         161.7         174.9  g.  anhydrous  salt, 

64.5°         85.60°      122° 

201.6  226.8        735.4  g.  anhydrous  salt. 
(Wolff,  Z.  anorg.  1905,  46.  94.) 


Very    deliquescent.      (Holz- 
mann, J.  pr.  84.  78.) 

Ammonium  cobalt  nitrate. 

Permanent.    Sol.  in  H2O.    (Thenard.) 

Ammonium  copper  nitrate,  2NH4N03, 

Cu(N03)2. 
Very  sol.  in  H2O. 

Ammonium    didymium    nitrate,    2NH4NO3, 

Di(NO3)3+4H2O. 
Somewhat  deliquescent. 

Ammonium   gadolinium  nitrate,   2NH4NO3, 

Gd(NO3)3. 
Deliquesces   in   the   air.      (Benedicks,    Z. 


liq 

:.  l 


anorg.  1900,  22.  407.) 

Ammonium  gold  (auric)  nitrate  (Ammonium 
auronitrate),  NH4Au(NO3)4. 

Extremely  deliquescent. 

H(NH4)2Au(NO3)6.  (Schottlander,  A.  217. 
312.) 

Ammonium   lanthanum   nitrate,    2NH4NO3, 

La(NO3)3+4H2O. 

Not  deliquescent.  Sol.  in  H2O.  (Marig- 
nac.) 


Ammonium  magnesium  nitrate,  2NH4NO3, 

Mg(N03)2. 

Slowly  deliquescent.  Sol.  in  10  pts.  H2O  at 
12.5°,  and  much  less  hot  H2O.  (Fourcroy.) 

Ammonium   mercurous   nitrate,    4NH4NO3, 

Hg,(NO,),+5H80. 
Sol.  in  H2O.     (Pagenstecher,  Reperfc.  14. 

188.) 

Ammonium  nickel  nitrate. 

Sol.  in  3  pts.  cold  H2O.  (Thenard,  Scher. 
J.  10.  428.) 

Ammonium  praseodymium  nitrate,  2NH4NO3, 

Pr(N03)3+4H20. 

Sol.  in  H2O.  (von  Scheele,  Z.  anorg.  1898, 
18.  356.) 

Ammonium  silver  nitrate,  NH4NO3,  AgNO3. 

Very  sol.  in  H2O.  (Russell  and  Maskelyne, 
Roy.  Soc.  Proc.  26.  357.) 

Sol.  in  H2O  without  decomp.  (Schreine- 
makers  and  de  Baat,  Chem.  Weekbl.  1910, 
7.6.) 

See  also  solubility  of  NH4NO3+AgNO3 
under  NH4NO3. 

Ammonium  thorium  nitrate,  (NH4)2Th(NO3)6. 

Sol.  in  strong  HNO3.  (Meyer,  Z.  anorg. 
1901,  27.  383.) 

NH4Th(NO3)5+5H2O.  Sol.  in  HNO3  of 
sp.  gr.  1.25.  (Meyer,  Z.  anorg.  1901,  27.  382.) 

Ammonium  uranyl  nitrate,  NH4NO3, 

U02(N03)2. 

Decomp.  by  H2O.  Sol.  in  cone.  HNO3. 
(Meyer,  B.  1903,  36.  4057.) 

Solubility  in  H2O  at  t°. 


t° 

In  100  pts.  by  wt. 
of  the  solution 

Solid  phase 

1  N 

*g 
a 

OH 

¥ 

£ 

flj 

•°  J 

00  ~O 

£*" 

0.5 
13.5 
24.9  a 
b 
35.0 
59.0 
80.7  a 
b 

29.71 
32.35 
36.40 
36.53 
42.07 
44.37 
44.90 
45.01 

2.92 
3.42 
3.54 
3.54 
3.44 
2.90 
2.98 
2.98 

68  '.72 
68.97 

78.76 
78.79 

Double  salt+UO2(NOs)i 
Double  salt 

Ammonium  uranyl  nitrate  is  decomp.  by 
H2O  at  temp,  below  60°:  above  60°  it  is  sol. 
in  H2O  without  decomp.  (Rimbach,  B.  1904, 
37.  475.) 

Ammonium  nitrate  ammonia,  2NH4NO3, 
3NH3. 

Known  only  as  a  solution  of  NH3  in 
NH4NO3+Aq.  (Troost,  C.  R.  94.  789.) 

NH4NO3,  3NH3.    As  above. 


552 


NITRATE,  AMMONIUM,  MERCURIC  CHLORIDE 


Ammonium  nitrate  mercuric  chloride, 

Solubility  in  100  pts.  H2O  at  t°. 

NH4NO3,  2HgCl2. 

Insol.  in  H2O.    Ether  dissolves  out  HgCl2. 

t 

Pts. 

Ba(NO3)2 

t° 

Pts. 
Ba(NO.). 

(Kosmann,  A.  ch.  (3)  27.  240.) 
2NH4NO3,   HgCl2.     Sol.  in  H2O.     (Hof- 

0 

5.0 

52 

17.7 

mann  and  Marburg,  A.  1899,  305.  199.) 

1 

5.1 

.  53 

18.1 

2 

5.3 

54 

18.4 

Ammonium     nitrate     sulphate,     2(NH4)2O, 

3 

4 

5.5 
5.7 

56 

18.7 
19.0 

N2O5,  2SO3,  H2O. 

5    ' 

6^0 

57 

19^3 

Very  hydroscopic  and  sol.  in  H20.    (Fried- 

6 

6.2 

58 

19.6 

heim,  Z.  anorg.  1894,  6.  297.) 
2NH4N03,  (NH4)2S04.    (de  Waal,  Dissert. 

7 
8 

6.4 
6.6 

59 
60 

20.0 
20.3 

1910.) 

9 

6.8 

61 

20.6 

3NH4NO3,  (NH4)2SO4.     (de  Waal.) 

10 

7.0 

62 

20.9 

See  also  solubility  of  NH4NO3+(NH4)2SO4 

11 

7.3 

63 

21.0 

under  NH4NO3. 

12 

7.5 

64 

21.6 

13 

7.7 

65 

21.0 

7  Q 

ftfi 

22  3 

Ammonium  nitrate  metotungstate,  NH4NO3. 

: 

15 

1    .  •' 

8.1 

\J\J 

67 

&+J  >  O 

22.6 

2(NH4)2W4013+4H20. 

16 

8^3 

68 

22.9 

Decomposes  by  recrystallising  out  of  H2O. 

17 

8.5 

69 

23.3 

(Marignac,  A.  ch.  (3)  69.  61.) 

18 

8.8 

70 

23.6 

19 

9.0 

71 

23.9 

Antimony  nitrate,  Sb4O6,  N2O5. 

21 

9.2 
9.5 

72 
73 

24  3 
24.9 

Decomp.  by  cold  H2O.    (Bucholz.) 

22 

9.7 

74 

25.0 

Aqueous  solution  sat.  at  10°  contains  30.4% 

23 

9.9 

75 

25.4 

salt.    (Eller.) 

24 

10.1 

76 

25.7 

Sol.  in  strong,  less  sol.  in  dil.  HNO3+Aq. 

25 

10.4 

77 

26.0 

(Peligot,  A.  ch.  (3)  20.  288.) 

26 

•  10.6 

78 

26.4 

Insol.  in  acetone.    (Naumann,  B.  1904,  37. 

27 

10.8 

79 

26.7 

4329.) 

28 

11.1 

80 

27.0 

29 

11.3 

81 

27.4 

OA 

HA 

82 

27  7 

Barium  nitrate,  Ba(NO3)2. 

31 

.  u 

11.8 

OH 

83 

I0f  «  4 

28.1 

Sol.  in  H2O  with  absorption  of  heat. 

32 

12.1 

84 

28.4 

100   pts.    H2O    at   0°    dissolve   5.0   parts 

33 

12.3 

85 

28.8 

Ba(NO3)2.    (Gay-Lussac,  A.  ch.  11.  313.) 

34 

12.6 

86 

29.1 

100   pts.    H2O    at   0°   dissolve   5.2    parts 

35 

12.8 

87 

29.5 

Ba(NO3)2.    (Mulder.) 

36 

13.1 

88 

29.8 

Ba(NO3)2+Aq  sat.  at  20°  contains  8.57  pts. 

37 

13.4 

89 

30.2 

Ba(NO3)2  to  100  pts.  H2O,  and  has  1.0679  sp. 

38 

13.7 

90 

30.6 

gr.  (Karsten);  sat.  at  20°  has  1.064  sp.  gr., 

39 

14.0 

91 

30.9 

and  contains  7.94  pts.  Ba(NO3)2  to  100  pts. 

40 

14.2 

92 

31.3 

H2O.    (Michel  and  Krafft.) 

41 

14.5 

93 

31.7 

42 

14.8 

94 

32.0 

100  pts.  H2O  dissolve  pts.  Ba(NO3)2  at  t°. 

43 
44 

15.1 
15.4 

95 
96 

32.4 
32.7 

0                              Pts                                   o                             PtS. 

45 

15.6 

97 

33.1 

Ba(N03)2                                  Ba(N03)2 

46 

15.9 

98 

33.5 

47 

1ft   9 

QQ 

qq   o 

0                 5.00            52.11          17.97 

rt/ 

48 

1O  .  ~i 

16.5 

yy 
100 

oo  .  o 

34.2 

14.95           8.18            73.75         25.01 

49 

16.8 

101 

34.5 

17.62           8.54            86.21         29.57 

50 

17.1 

101.9 

34.8 

37.87          13.67           101.65          35.18 

51 

17.4 

40  29           17  07 

T^t/.X'jj                     JL  1    .  V/l                                  ...                               ... 

(Moulder   calculated  from  his  own  and  other 

(Gay-Lussac,  A.  ch.  (2)  11.  313.) 

experiments,   Scheik.  Verhandel.   1864.   50.) 

NITRATE,  BARIUM 


553 


Sat.   Ba(NO3)2+Aq   contains    %   Ba(NO3) 
at  t°. 


0.4 

2.1 

6.0 

6.5 

11.0 

15.3 

18.0 

28.5 

45.5 

52.0 


Ba(NO.)2 


4.3 
4.9 

5.6 

5.6 

6.4 

7.1 

7.7 

9.7 

12.8 

14.9 


60.0 

73.0 

92.0 

110.0 

132.0 

134.0 

150.0 

152.0 

171.0 

215.0 


% 

Ba(i\08). 


16.1 
19.4 
23.4 
27.4 
31.8 
32.5 
34.9 
35.4 
38.3 
45.8 


(Etard,  A.  ch.  1894,  (7)  2.  528.) 

100  g.  H2O  dissolve  8.54  g.  Ba(NO3)2  at 
17°.  (Gmelin-Kraut,  Handbuch  der  anorg. 
Chemie.) 

100  g.  H2O  dissolve  7.87  g.  Ba(N03)2  at 
15°;  8.32  g.  at  17°.  (Euler,  Z.  phys.  Ch.  1904, 
49.  315.) 

1000  g.  H2O  dissolve  0.72  gram-equivalents 
Ba(NO3)2  at  21.5°.  (Euler,  Z.  phys.  Ch 
1904,  49.  312.) 

10.30  g.  anhydrous  Ba(NO,)2  are  sol.  in 
100  g.  H2O  at  25°.  (Parsons  and  Colson,  J. 
Am.  Chem.  Soc.  1910,  32.  1385.) 

4.74  g.  Ba(NO3)2  are  contained  in  100  g. 
Ba(NOj)2  sat.  at  0°.  (Coppadoro,  Gazz.  ch. 
it.  1911,  42,  I.  233.) 

Solubility  of  Ba(NO3)->  in  H2O  =0.427  mol. 
1.  at  30°.  (Masson,  Chem.  Soc.  1911,  99. 
1136.) 

Solubility  of  Ba(NO3)2  in  H2O  at  30°  = 
10.33%.  (Coppadoro,  Gazz.  ch.  it.  1913,  43. 
I.  240.) 

Solubility  in  H2O. 

100  g.  of  the  sat.  solution  contain  at: 

9.1°         21.1°          35° 

6.25        8.46          11.39  g.  Ba(NO3)2. 

(Findlay,  Chem.  Soc.  1914,  105.  780.) 
Sp.  gr.  of  Ba(NO3)2+Aq  at  19.5°. 


Sp.gr.  of  Ba(NO3)2+Aq  at  17.5°. 


m 
Ba(NO8)2 

Sp.  gr. 

Ba(tfOi)» 

Sp.  gr. 

1 

2 
3 
4 
5 

1.0085 
1.0170 
1.0255 
1.0340 
1.0425 

6 
7 
8 
Sat.  sol. 

1.0510 
1.0600 
1.0690 
1.0690 

(Gerlach,  Z.  anal.  27.  283.) 
Sp.  gr.  of  Ba(NO3)2-fAq  at  room  temp. 


%  Ba(NOr)i 


5.25 
2.98 


Sp.  gr. 


1.0507 
1.0274 


(Wagner,  W.  Ann.  1883,  18.  264.) 
Sp.  gr.  of  Ba(NO,)2+Aq  at  25°. 


Concentration  of 
Ba(NOs)2+Aq. 


V2  normal 


Sp.  gr. 


1.0518 
1.0259 
1 . 0130 


(Wagner,  Z.  phys.  Ch.  1890,  6.  35.) 

Ba(NO3)2+Aq  containing  6.08%  Ba(NO3)2 
has  sp.  gr.  20° /20°  =  1.0517. 

Ba(NO3)2+  Aq  containing  6.97%  Ba(NO3)2 
has  sp.  gr.  20°/20°  =  1 .0597. 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  279.) 

Sp.  gr.  of  Ba(NO3)2+Aq  at  20°  containing 
M  g.  mols.  salt  per  liter. 


M 
Sp.  gr. 


0.01 
1.002031 


0.025 
1.005224 


0.05 
1.010591 


M      0.075      0.10       0.15 
Sp.  gr.   1.015671    1.021143    1.031770 
(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38.  708.) 


Ba(jfo3)2 

Sp.  gr. 

Ba(N03)2 

Sp.  gr. 

Sp.  gr.  ot  sat.  i*a(W03)2+Aq  at  t°. 

t° 

g.  Ba(NOi)isol. 
in  100  g.  H2O 

Sp.  gr. 

1 

2 

3 
4 
5 

.009 
.017 
.025 
.034 
.042 

6 
7 
8 
9 
10 

1.050 
1.060 
1.069 
1.078 

1.087 

0 
10 
20 
30 
40 
50 
60 
70 

5.2 
7.0 
9.2 
11.6 
14.2 
17.1 
20.3 
23.6 

1.043 
1.056 
.073 
.087 
.104 
.121 
.137 
.146 

(Calculated  by  Gerlach,  Z.  anal.  8.  286,  from 
Kremers,  Pogg.  95.  110.) 

Sp.  gr.  of  Ba(NO3)2+Aq  at  18°. 

%  Ba(N03)2 

Sp.  gr. 

Tschernaj,  J.  Russ.  Phys.  Chem.  Soc.  1912, 
44.  1565.) 

Saturated  BaNO3+Aq  contains:— 
36.18  pts.  Ba(NO3)2  to  100  pts.  H2O,  and 
boils  at  101.1°.    (Griffiths.) 

4.2 

8.4 

1.0340 
1.0712 

(Kohlrausch,  W.  Ann.  1879.  1.) 

554 


NITRATE,  BARIUM 


35.2  pts.  Ba(NO3)2  to  100  pts.  H2O,  and 
boils  at  101.65°.  (Gay-Lussac.) 

34.8  pts.  Ba(NO3)2  to  100  pts.  H2O,  and 
boils  at  101.9°.  (Mulder.) 

34.8  pts.  Ba(NO3)2  to  100  pts.  H2O,  and 
boils  at  102.5°.  (Kremers.) 

Sat.  Ba(NO3)2+Aq  forms  a  crust  at  101.1°; 
highest  temp,  observed  was  101.5°.  (Gerlach, 
Z.  anal.  26.  427.) 

B.    pt.    of    Ba(NO3)2+Aq    containing    pts. 
Ba(NO3)2  to  100  pts.  H2O. 


B.-pt. 

Pts.  Ba(NO3)2 

100.5° 
101.0 
101  .  1 

12.5 
26.0 
27.5 

(Gerlach,  Z.  anal.  26.  440.) 

Insol.  in  cone.  HNO3+Aq,  and  much  less 
sol.  in  dil.  HNO3+Aq  or  HCl+Aq  than  in 
H2O. 


13.67  pts.  NH4Cl+Aq  (1  pt.  NH4C1+10 
pts.  H2O)  at  ord.  temp.,  and  4.67  pts.  at 
100°. 

24.00  pts.  NH4NO3+Aq  (1  pt.  NH4NO3  + 
10  pts.  H2O)  at  ord.  temp. 

17.33  pts.  Nri4C2H3O2+Aq  (dil.  NH4OH 
neutralised  by  dil.  HC2H3O2)  at  ord.  temp., 
and  4.33  pts.  at  100°. 

14.67  pts.  NaC2H3O2+Aq  (dil.  HC2H3O2 
neutralised  by  Na2CO3  and  dil,  with  4  vols. 
H2O)  at  ord.  temp.,  and  5.33  pts.  at  100°. 

17.33  pts.  Cu(C2H3O2)2+Aq  (see  Stolba,  Z. 
anal.  2.  390)  at  ord.  temp.,  and  6.00  pts.  at 
100°. 

18.67  pts.  grape  sugar  (1  pt.  grape  sugar 
+10  pts.  H20)  at  ord.  temp.  (Pearson,  Zeit. 
Ch.  1869.  662.) 

Sol.  in  sat.  NH4Cl+Aq  without  pptn.  at 
first,  but  finally  NH4C1  is  pptd.  until  a  cer- 
tain state  of  equilibrium  is  reached.  (Kar- 
sten.) 

Solubility  in  BaO2H2,  8H2O+Aq  at  25°. 


Solubility  of  Ba(NO3)2  in  HNO3+Aq  at  30°. 

Sp.  gr.  25°/25° 

G.  BaO  as 
Ba(OH)2  in 

1  f\f\     re        XT     (~\ 

G.  Ba(N03)2 
in  100  g.  H20 

Solid  phase  Ba(NO3)2 

1UU     g.     ±12U 

i   07Q7 

o 

10  "30 

G.  mol.  per  1. 

X  .  \J  t  t7  1 

1  .  1002 

\J 

1.55 

JL\J  .  OLF 

10.66 

Sp.  gr.  of  sat. 

1.1210 

3.22 

11.04 

HNOs 

Ba(NO3)2 

*1  .  1448 

5.02 

11.48 

1.0891 
1.0811 

l!o663 

0.0000 

0.1318 
0.2496 
0.4995 

0.4270 
0.3282 
0.3268 
0.2410 

*  This  solution  is  sat.  with  respect  to  both 
Ba(OH)2,  8H2O  and  Ba(NO3)2. 
(Parsons.   J.  Am.  Chem.  Soc.  1910,  32.  1385.) 

1.0619 

0.7494 

0.1785 

See  also  under  BaO2H2. 

.0609 

1.000 

0.1353 

.0633 
.0668 

1.247 
1.493 

0.1056 
0.0847 

Solubility  in  BaCl2+Aq  at  t°. 

.0783 

1.998 

0.0598 

Sat.  solution  contains 

.1050 

2.993 

0  0334 

t° 

1.1341 

3.986 

0.0218 

%  BaCl2 

%  Ba(N03)2 

1.1341 

3.994 

0.0223 

1.1645 

5.012 

0.0147 

n 
J 

21.4 

00     A 

4.0 

4-  0 

(Masson,  Chem.  Soc.  1911,  99.   1136.) 

+1.5 

£d  .  \J 

22.6 

TT  .  \J 

4.4 

2 

5.0 

Less  sol.  in  dil.  HC2H3O2+Aq  than  in  dil. 
HCl+Aq. 

10 
21 

24^7 
24.5 

6.1 
5.6 

Solubility  in  NH4Cl+Aq  is  the  same  as  in 

32 

26.6 

7.7 

H2O. 

35 

26.4 

7.7 

Less  sol.  in  NH4OH+Aq,  NH4C2H3O2  + 
Aq,  or  NH4NO3  +  Aq  than  in  H2O.    (Pearson, 
Zeit.  Ch.  (2)  6.  662.) 

38 
48 
53 

26.7 
28.1 

28.5 

7.8 
8.0 
9.0 

Ba(NO3)2  is  sol.  in  about: 

53 

28.3 

9.2 

13.33  pts.  H2O  at  ord.  temp.,  and  4.67  pts. 

66 

28.0 

10.0 

at  100°. 

73 

30.0 

10.5 

14.67   pts.    NH4OH+Aq    (cone.)    at   ord. 

79 

30.3 

11.2 

temp.,  and  5.67  pts.  at  100°. 

90 

32.1 

12.5 

16.50  pts.  NH4OH+Aq  (1  vol.  cone.  +3 

155 

32.5 

23.1 

vols.  H2O)  at  ord.  temp. 

162 

33.1 

23.4 

28.00  pts.  HCl+Aq  (1  vol.  cone.  HC1+4 

210 

32.5 

31.9 

vols.  H2O)  at  ord.  temp. 
29.00  pts.  HC2H3O2+Aq  (1  vol.  commer- 
cial HC2H3O2  +  1  vol.  H2O)  at  ord.  temp. 

(fitard,  A.  ch.  1894,  (7)  3.  287.) 
See  also  under  BaCl2. 

NITRATE,  BARIUM 


555 


Ba(N03)2+Pb(NO3)2. 

Very  si.  sol.  in  sat.  Pb(NO3)2+Aq.  (Kar- 
sten.) 

100  pts.  sat.  Ba(NO3)2+Pb(NO3)2+Aq 
contain  33.95  pts.  of  the  two  salts  at  19-20°. 
(v.  Hauer,  J.  pr.  98.  137.) 

Solubility  of  Ba(N03)2+Pb(N03)2  at  25°. 


J                                        01^ 

G.  ] 

Der  1. 

Sp.  gr. 

100  pt 

3.   Of  SOlu- 

Ba(N03)2 

Pb(NO»)i 

tion 

contain 

Solid  phase 

102.2 

0 

.079 

pts. 
KNOs 

pts. 
Ba(NOs)2 

54  9 

17  63 

088 

86.5 

49.80 

.108 

15.24 

6.64 

Ba(NO3)2+2KNO3,  Ba(NO3)2 

79.7 

68.10 

.119 

14.69 

6.60 

it 

77.0 

97.20 

.140 

14.79 

6.62 

tt 

69.8 
66.0 

130.7 
177.3 

.163 
.198 

16.30 
21.99 

5.49 
3.04 

2KN03,  Ba(N03)2 
tt 

57.5 
25.9 

247.7 
334.3 

.252 
.294 

27.66 

27.81 

2.01 
2.09 

KNO3+2KNO3,  Ba(NO3)2 

a 

28.8 

429.7 

.376 

27.94 

1.92 

(f 

0 

553.8 

1.459 

27.64 

2.05 

(t 

(Fock,  Z.  Kryst.  Min.  1897,  28.  365,  397.) 

100  ccm.  Ba(N03)2+Pb(NO3)2+Aq  sat. 
at  17°  contain  3.22  g.  Ba(NO3)2  and  38.59  g. 
Pb(N03)2  and  solution  has  sp.  gr.  =  1.350. 
(Euler,  Z.  phys.  Ch.  1904,  46.  313.) 

100   pts.   sat,    Ba(NO3)2+Pb(NO3)2  + 
Sr(NO3)2+Aq  contain  45.90  pts.  of  the  three 
salts  at  19-20°.    (v.  Hauer,  1.  c.) 

Ba(N03)2+Sr(N03)2. 

100  pts.  sat.  Ba(NO3)2+Sr(NO3)2+Aq  con- 
tain 45.96  pts.  of  the  two  salts  at  19-20°. 
(v.  Hauer,  I.  c.) 

Ba(N03)2+KNO3. 

100  pts.  H2O  dissolve: 


(Mulder) 

(1) 

KNO3  . 

Ba(N03)2  .      . 

29.7 

28.8 
5.4 

8^9 

34.2 

(Karsten) 

(Kopp) 

(4)   '  (5) 

(2)           (3) 

KNO3 

Ba(N03)2     . 

13.31 
6.91 

29.03 
1.00 

5.7 
33.1 

3.5 
36.3 

20.22 

30.03 

38.8 

39.8 

1.  Sat.  Ba(NO3)2+Aq  sat.  with  KNO3  at 
18.5°. 

2.  To  sat.  KNO3+Aq,  Ba(NO3)2+Aq  was 
added. 

3.  To    sat.    Ba(NO3)2+Aq,     KNO3    was 
added. 

4.  Both  salts  in  excess +Aq  at  21.5°. 

5.  Both  salts  in  excess -f-Aq  at  23°. 


1 1.  of  the  solution  contains  59.1  g.  Ba(NO3)2 
+124.2  g.  KNO3  =  183.35  g.  mixed  salts  at 
17°.  Sp.  gr.  Ba(NO3)2+KNO3+Aq  =  1.120. 

1 1.  of  the  solution  contains  88.7  g.  Ba(NO3)2 
+213.6  g.  KNO3  =  302.3  g.  mixed  salts  at 
30°.  Sp.  gr.  Ba(NO3)2+KNO3+Aq  =  1.191. 
(Euler,  Z.  phvs.  Ch.  1904,  49.  313.) 


These  results  show  that  a  double  salt  of 
potassium  and  barium  nitrates  is  formed  at 
25°. 

(Foote,  Am.  Ch.  J.  1904,  32.  252.) 

Solubility  of  Ba(NO3)2+KNO3  at  t°. 


t° 

Ba(NOs)2 

% 

KNOs 

Solid  phase 

9.1 

6.25 

0 

Ba(N03)2 

4.20 

8.15 

Ba(NO3)2+2KNO3, 

Ba(N03)2 

1.98 
0.98 

12.02 
16.80 

2KNO3,  Ba(NO3)2 
2KN03,  Ba(N03)2+ 
KNO3 

0 

16.76 

KNO3 

21.1 

8.46 

0 

Ba(N03)2 

7.47 

2.12 

" 

6.35 

5.98 

" 

6.06 

8.47 

Cl 

5.98 

13.24 

Ba(NO3)2+2KNO3, 

Ba(N03)2 

3.35 

18.24 

2KNO3,  Ba(NO3)2 

2.30 

21.47 

tt 

1.76 

24.86 

2KN03,  Ba(N03)2+ 
KNO3 

0 

24.77 

KNO3 

35 

11.39 

0 

Ba(N03)2 

8.18 

12.99 

" 

8.08 

17.48 

H 

8.42 

19.75 

Ba(NO3)2+2KNO3, 

Ba(NO3)2 

5.85 

24. 

2KN03,  Ba(N03)2 

5.02 

26.05 

1C 

3.02 

34.87 

2KNO3,  Ba(NO3)2+ 

KNO3 

1.77 

34.98 

KNO3 

0 

35.01 

it 

(Findlay,  Chem.  Soc.  1914,  105.  779.) 


556 


NITRATE,  BARIUM 


Ba(NO.)H-NaNO«. 

Ba(NO3)?  is  sol.  in  sat.  NaNO3+Aq  with- 
out separation. 

100  pts.  H2O  dissolve: 


NaNO3 
Ba(NO,),      .      .      . 

(Karsten) 
At  18.75° 

86.6 

88.14 
3.77 

8^9 

NaNO, 

Ba(N03)2       .      .      . 

(Kopp) 
At  20.2° 

87.7 

88.6 
3.6 

M 

Solubility  of  Ba(NO3)2+NaNO3  in  H2O  at  0°. 


%  NaNOs 

%  Ba(NOs)* 

Solid  phase 

0 

4.74 

Ba(N03)2 

0.41 

4.33 

0.61 

4.03 

K 

1.68 

3.34 

<( 

3.54 

2.50 

(( 

8.05 

1.60 

t( 

12.71 

1.56 

u 

20.24 

1.53 

u 

2CK92 

1.43 

u 

27.74 

1.56 

a 

30.81 

1.55 

a 

33.79 

•    1.53 

it 

35.83 

1.49 

it 

41.30 

1.55 

Ba(NO3)2+NaNO3 

41.68 

0.51 

NaNO3 

42.47 

0 

u 

(Coppadoro,  Gazz.  ch.  it,  1912,  42  (1)  233.) 

Solubility  of  Ba(NO3)2+NaNO3  in  H2O 
at  30°. 


% 

NaNOs 

• 

Ba(NOs)2 

Solid  phase 

0 

10.33 

Ba(N03)2 

2.33 

8.58 

7.09 

5.28 

12.07 

3.89 

14.41 

3.54 

17.87 

3.20 

19.06 

3.07 

23.55 

2.81 

41.22 

2.27 

48.22 

2.11 

Ba(NO3)2+NaNO3 

48.50 

1.00 

NaNO3 

49.16 

0 

it 

(Coppadoro,  Gazz.  ch.  it.  1013,  43,  I.  240.) 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  827.) 

100  pts.  hydrazine  dissolves  81.1  pts. 
Ba(NO3)2  at  12.5-13°.  (de  Bruyn,  R.  t.  c. 
1899,  18.  297.) 


100  pts.  anhydrous  hydroxylamine  dissolve 
11.4  pts.  Ba(NO3)2.  (de  Bruyn,  R.  t.  c. 
1892,  11.  18.) 

Insol.  in  absolute  alcohol. 

Solubility  in  dilute  alcohol  increases  with 
the  temp.  (Gerardin,  A.  ch.  (4)  5.  145.) 

Solubility  in  ethyl  alcohol +Aq  at  25°. 


%  C2H5OH  in 
the  solvent 

%  C2H5OH  in 
the  solution 

%  Ba(N03)2in 
the  solution 

0 

0 

9.55 

10.25 

9.5 

7.63 

18.60 

17.5 

6.02 

25.05 

23.7 

5.25 

40.20 

38.8 

3.53 

58.00 

57.0 

1.85 

78.70 

78.2 

0.62 

90.10 

89.9 

0.18 

99.40 

99.39 

0.005 

(D'Ans  and  Siegler,  Z.  phys.  Ch.  1913,  82. 37.) 

Completely  insol.  in  boiling  amyl  alcohol. 
(Browning,  Sill.  Am.  J.  143.  314.) 

Solubility  in  organic  solvents. 


Solvent 


Methyl  alcohol 
Ethyl  alcohol 
Acetone 
Ether 
Paracetaldehyde 


%  Ba(NO3)2in  the 
solution  at  25° 


0.50 
0.005 
0.005 
very  small 


(D'Ans  and  Siegler,  Z.  phys.  Ch.  1913,  82. 44.) 
Solubility  in  phenol  +Aq  at  25°. 


Concentration  of  the  phenol 
Mol./ Liter 


0.000 
0.045 
0.082 
0.146 
0.310 
0.401 
0.501 
0.728  (sat.) 


Solubility  of  Ba(NOs)  2 
Mol./Liter 


0.3835 
0.3785 
0.3746 
0.3664 
0.3492 
0.3400 
0.3299 
0.3098 


(Rothmund  and  Wilsmore,  Z.  phys.  Ch.  1902, 
40.  620.5 

Insol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1370.) 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1904,  37.  3602.) 

Insol.  in  acetone.  (Krug  and  M'Elroy,  J. 
Anal.  Ch.  6.  184.) 

Difficultly  sol.  in  acetone.  (Naumann,  B. 
1904,  37.  4328.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899,  II. 
1014.) 


NITRATE,  BISMUTH  MANGANOUS 


557 


Barium   mercurous   nitrate,   2BaO,   2Hg2O, 

3N2O5. 

Decomp.  by  H2O.  Sol.  in  hot  dil.  HNO3+ 
Aq  and  hot  Hg2(NO3)2+Aq,  from  which  it 
crystallises  on  cooling.  (Stadeler,  A.  87.  129.) 

Barium  potassium  nitrate,  Ba(NO3)2,  2KNO3. 

Ppt.  (Wallbridge,  Am.  Ch.  J.  1903,  30. 
154.) 

Solubility  determinations  show  that  the 
only  double  salt  formed  by  barium  and 
potassium  nitrates  at  25°  is  Ba(NO3)2, 2KNO3. 

See  Ba(NO3)2+KN03  under  Ba(NO3)2. 
(Foote,  Am.  Ch.  J.  1904,  32.  252.) 

Barium    nitrate    raetatungstate,    2Ba(NO3)2. 

BaW4013+6H20. 

Efflorescent.  Sol.  in  warm  H2O.  (Pe"ch- 
ard,  A.  ch.  (6)  22.  198.) 

Bismuth  nitrate,  basic,  Bi2O3,  N  2O5+2H2O. 

Sol.  in  a  large  amount  of  H2O.  Sol.  in 
HNO3+Aq.  (Heintz.) 

Sol.  in  135  pts.  H2O  at  90-93°.  (Ruge,  J.  B. 
1862.  163.) 

+  ^H2O.  Sol.  in  much  H2O.  (Yvon, 
C.R.  84.  1161.) 

+H2O.    (Ruge.) 

2Bi2O3,  N2O6.  Not  acted  upon  by  H2O. 
(Ditte,  C.  R.  84.  1317.) 

+H2O.    (Yvon.) 

Bi2O3,  2N2O5+H2O.     (Ruge.) 

HBi2O3,  5N2O5+16H2O.  Not  decomp.  by 
H2O.  (Yvon.) 

5Bi2O3,  4N2O5+8H2O.  Ppt.  Not  attacked 
by  H2O.  (Schulten,  Bull.  Soc.  1903,  (3)  29. 
722.) 

5Bi2O3,  5N2O5+9H2O.  Sol.  in  H2O  with 
decomp.  (Schulten.) 

6Bi2O3,  5N2O5+8H2O,  and  +9H2O.  (Rut- 
ten,  Z.  anorg.  1902,  30.  368.) 

At  25°  the  salt  Bi12O13(NO3)io,  9H2O  is  in 
equilibrium  with  HNO3+Aq  from  0.03- 
0.32-N;  the  salt  BiO(NO3),  H2O  is  in  equi- 
librium with  HNO3+Aq  from  0.425-0.72-N. 

At  50°  the  salt  Bi4O6(NO3)2,  H2O  is  in 
equilibrium  with  HNO3+Aq  from  0.057- 
0.285-N;  the  salt  Bi12Oi3(NO3)io,  9H2O  is  in 
equilibrium  with  HNO3+Aq  from  0.285- 
0.446-N. 

At  75°  the  salt  Bi4O6(NO3)2,  H2O  is  in 
equilibrium  .with  HNO3+Aq  from  0.109- 
0.314-N.  (Allan,  Am.  Ch.  J.  1901,  25.  314.) 

Bismuth  nitrate,  Bi(NO3)3. 

Permanent.  Decomp.  by  little  H2O  with 
separation  of  a  basic  salt:  This  decomposition 
is  prevented  by  slight  excess  of  HNO3,  and 
then  the  salt  is  completely  sol.  in  a  large 
amount  of  H2O.  (Rose.) 

Sol.  in  dil.  HNO3+Aq.  Not  decomp.  by 
H2O  in  presence  of  HC2H3O2  or  ^fa  pt. 
NH4NO3.  (Lowe,  J.  pr.  74.  341.) 

Completely  sol.  in  HNO3+Aq  containing 
83  g.  HNO3  per  liter.  (Ditte.) 


Solubility  of  Bi(NO3)3  in  2.3N-HNO3+Aq. 
=  2.04  g.  at  Bi  per  1.;  in  0.922N-HNO3+Aq. 
=  2.23  g.  at  Bi  per  1.  (Dubrisay,  C.  R.  1911. 
153.  1077.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

Insol.  in  acetone.    (Krug  and  M'Elroy.) 

Solubility  of  Bi(NO3)3  in  6.67%  acetone+ 
2.3N-HNO3+Aq  =  1.89  g.  at  Bi  per  1.;  in 
6.67%  acetone +0.922N-HNO3+Aq.  =2.17  g. 
at  Bi  per  1.;  in  13.33%  acetone +0.922N- 
HNO3+Aq  =2.08  g.  at  Bi  per  1.  (Dubrisay, 
C.  R.  1911,  153.  1077.) 

When  Bi(NO3)3-is  mixed  with  mannite 
(dulcite,  sorbite)  in  proportion  to  the  mol. 
wts.  and  H2O  is  added,  a  clear  solution  is  ob- 
tained which  is  not  pptd.  by  addition  of 
much  H2O.  These  solutions  are  more  stable 
the  greater  the  proportion  of  mannitol. 
(Vanino  and  Hunser,  Z.  anorg.  1901,  28.  211.) 

+  1^H2O.    (Ditte.) 

+5H2O.  If  treated  with  increasing  amts. 
of  H2O,  the  amt.  of  Bi  which  dissolves  de- 
creases, and  when  1  pt.  is  treated  with 
50,000  pts.  H2O,  no  Bi  goes  into  solution. 
(Antony  and  Gigli,  Gazz.  ch.  it.  1898,  28. 
245.) 


48.66  pts.  are  sol.  in  100  pts.  acetone  at    0°. 
41.70     "    "     "    "  100    "        "         "  19°. 
(Laszczynski,  B.  1894,  27.  2287.) 

+5^H2O.    (Yvon,  C.  R.  84.  1161.) 
+  10H2O.     Melts  in  crystal  H2O  with  de- 
comp. at  74°.    (Ordway.) 

Bismuth  caesium  nitrate,  Bi(NO3)3,  2CsNO3. 
Ppt.    (Wells,  Am.  Ch.  J.  1901,  26.  277.) 

Bismuth  cobalt  nitrate,  2Bi(NO3)3,  3Co(N03)2 

+24H2O. 

100  cc.  sat.  solution  in  HNO3+Aq  (sp.  'gr. 
1.325)  contain  54.67  g.  hydrated  salt.  (Jantsch 
Z.  anorg.  1912,  76.  321.) 

Bismuth  magnesium  nitrate,  2Bi(NO3)3, 
3Mg(NO3)2+24H2O. 

Deliquescent.  Effloresces  in  dry  air. 
Decomp.  by  H2O.  (Urbain  and  Lacombe, 
C.  R.  1903,  137.  569.) 

100  cc.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contain  41.69  g.  hydrated  salt.  (Jantsch 
Z.  anorg.  1912,  76.  321.) 

Bismuth  manganous  nitrate,  2Bi(NO3)3, 
3Mn(NO3)2+24H2O. 

Deliquescent.  Effloresces  in  dry  air. 
Decomp.  by  H2O.  (Urbain  and  Lacombe. 
C.  R.  1903,  137.  569.) 

100  cc.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contain  65.77  g.  hydrated  salt.  (Jantsch 
Z.  anorg.  1912,  76.  321.) 


558 


NITRATE,  BISMUTH  NICKEL 


Bismuth  nickel  nitrate,  2Bi(NO3)3,  3Ni(NO3)2 
+24H2O. 

Deliquescent.  Effloresces  in  dry  air. 
Decomp.  by  H2O.  (Urbain  and  Lacombe, 
C.  R.  1903,  37.  569.) 

100  cc.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contain  46.20  g.  hydrated  salt  at  16°. 
(Jantsch.) 

Bismuth  zinc  nitrate,  2Bi(NO3)3,  3Zn(NO3)2  + 
24H2O. 

Deliquescent.  Decomp.  by  H2O.  (Ur- 
bain and  Lacombe,  C.  R.  1903,  137.  569.) 

100  cc.  sat.  solution  in  JENO3+Aq  (sp.  gr. 
1.325)  contain  57.51  g.  hydrated  salt  at  16°. 
(Jantsch.) 

Cadmium  nitrate,  basic,  Cd(OH)NO3+H2O. 

Decomp.  by  H2O,  or  ordinary  alcohol. 
(Klinger,B.  16.997.) 

12CdO,  N205+11H20.  SI.  sol.  in  H2O; 
more  sol.  in  H2O  than  basic  sulphate.  (Haber- 
mann,  5.  432.) 

5  CdO,  2N2O6-f8H2O.  Decomp.  by  cold 
H2O.  (Rousseau  and  Tite,  C.  R.  114.  1184.) 

Cadmium  nitrate,  Cd(N03)2. 

Deliquescent,  and  very  sol.  in  H2O. 
See  +4,  and  9H2O. 

Sp.  gr.  of  aqueous  solution  containing: 
5         10         15         20        25%Cd(NO3)2, 
1.0528  1.0978  1.1516  1.2134  1.2842 

30        35        40        45        50%Cd(NO3)2. 
1.3566  1.4372  1.5372  1.6474  1.7608 
(Franz,  J.  pr.  (2)  5.  274.) 

Sp.  gr.  of  Cd(NO3)2+Aq  at  18°. 
%Cd(NO3)2        1  5  10  15 

Sp.gr.  1.0069     1.0415     1.0869     1.136 

Cd(NO3)2        20          25         30  35 

.  gr.  1.1903     1.25     1.3125     1.3802 

Cd(NO3)2       40  45  48 

p.  gr.  1.459       1.543       1.5978 

(Grotrian,  W.  Ann.  1883,  18.  193.) 

Sp.gr.  of  Cd(NO3)2+Aq  at  room  temp, 
containing: 

7.81         15.71        22.36%  Cd(NO3)2. 
1.0744       1.1593       1.2411 
(Wagner,  W.  Ann.  1883,  18.  265.) 

Sp.gr.  of  Cd(N03)2+Aq. 


% 

Cd(NO3)2 

"t 

Sp.  gr.  at  t° 

Sp.  gr.  at  18° 

0.0492 

17.57 

0.99912 

0.99904 

21.14 

0.99839 

0.100 

18.00 

0.99945 

0.249 

17.34 

1.0008 

1.0007 

20.22 

1.0002 

0.464 

18.00 

1.0025 

0.952 

18.00 

1.0065 

(Wershofen,  Z.  phys.  Ch.  1890,  5.  493.) 


Sp.  gr.  of  Cd(NO3)2+Aq  at  25°. 


Concentration  of 
Cd(NOs)2+Aq. 


1-normal 

Vr-     " 


Sp.  gr. 


1.0954 
1.0479 
1.0249 
1.0119 


(Wagner,  Z.  phys.  Ch.  1890,  6.  36.) 

Sp.  gr.  of  Cd(NO3)2+Aq  at  18°/4°. 
%Cd(NO3)2        54.027        43.716         30.879 
Sp.gr.  1.711          1.515          1.321 

%Cd(NO3)2        21.353         14.899          8.683 

Sp.  gr.  1.204          1.134  1.074 

(de  Muynck,  W.  Ann.  1894,  53.  561.) 

Cd(NO3)2+Aq  containing  7.89%  Cd(NO3)2 
has  sp.  gr.  20°/20°  =  1.0673. 

Cd(NO3)2  +  Aq  containing  12.14% 
Cd(NO3)2  has  sp.  gr.  20°/20°  =  1.1070. 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  282.) 

Sat.  Cd(NO3)2+Aq  boils  at  132°. 

Almost  entirely  insol.  in  cone.  HNO3-fAq. 
(Wurtz.) 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  827.) 

Sol.  in  alcohol. 

Sol.  in  ethyl  acetate.  (Naumann,  B.  1904, 
37.  3601.) 

Sol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

+4H2O.  M.-pt.  of  Cd(NO3)2-HH2O  = 
59.5°.  (Ordway;  Tilden,  Chem.  Soc.  45.  409.) 

Solubility  in  H2O. 

Solubility  in  H2O  at  t°. 


t° 

%  Cd(NO?)2  in 
the  solution 

Mols.  H2O  to 
1  mol.  Cd(NO3)2 

0 
18 
30 
40 
59.5  mpt. 

52.31 
55.90 
58.40 
61.42 
76.54 

11.96 
10.34 
9.34 

8.24 
4.00 

(Funk,  B.  1899,  32.  105.) 

Sat.  solution  of  Cd(NO3)2+4H2O  in  H2O 
at  0°  contains  52.3%  Cd(NO3)2;  at  18°, 
55.9%  Cd(NO3)2.  (Mvlius,  Z.  anorg.  1912, 
74.  411.) 

Sol.  in  liquid  NH3.  (Johnson  and  Wils- 
more,  Elektroch.  Z.  1908,  14.  227.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

Sol.  in  ethyl  acetate.  (Naumann,  B.  1910, 
43.  314.) 

+9H2O.    Solubility  in  H2O. 

Sat.  solution  contains  at: 
—13°  —1°  +1° 
37.37  47.33  52.73%  Cd(NO3)2. 


NITRATE,  CALCIUM 


559 


Cryohydrate  is  formed  at  — 16°.  (Funk, 
Z.  anorg.  1899,  20.  416.) 

The  composition  of  the  hydrates  formed  by 
Cd(NO3)2  at  different  dilutions  is  calculated 
from  determinations  of  the  lowering  of  the 
fr.-pt.  produced  by  Cd(NOs)2  and  of  the  con- 
ductivity and  sp.  gr.  of  Cd(NO3)2+Aq. 
(Jones,  Am.  Ch.  J.  1905,  34.  308.) 

Cadmium  uranyl  nitrate,  Cd(NO3)2, 

(UO2)(NO3)2+30H2O. 
Sol.  in  H2O  and  acids.     Insol.  in  alcohol 
and  alkalies +Aq.     (Lancien,  C.  C.  1912.  1. 

208.) 

Cadmium  nitrate  ammonia.  Cd(NO3)2,  6NH3 

+H20. 
(Andre,  C.  R.  104.  987.) 

Cadmium   nitrate   cupric   oxide,   Cd(NO3)2, 

CuO+5H2O. 
Ppt.    (Mailhe,  C.  R.  1902,  134.  235.) 

Cadium  nitrate  cupric  oxide,  Cd(NO3)2, 
3CuO+5H2O. 
(Mailhe,  A.  ch.  1902,  (7)  27.  383.) 

Cadmium  nitrate  hydrazine,   Cd(NO3)2, 

3N2H4. 

Decomp.  by  hot  H2O.  Sol.  in  warm 
NH4OH.  (Franzen,  Z.  anorg.  1908,  60.  282.) 

Caesium  nitrate,  CsNO3. 

100  pts.  H2O  dissolve  10.58  pts.  CsNO3  at 
3.2°.  SI.  sol.  in  absolute  alcohol.  (Bunsen.) 
h. 

Solubility  of  CsNO3  in  H2O  at  t°. 


t° 

G.  CsNOs 
per  100  g. 

t 

G.  CsNOa 
per  100  g. 

Solu- 
tion 

Water 

Solu- 
tion 

Water 

0 
10 
20 
30 
40 
50 

8.54 
12.97 
18.7 
25.3 
32.1 
39.2 

9.33 
14.9 
23.0 
33.9 
47.2 
64.4 

60 
70 
80 
90 
100 
106.2 

45.6 
51.7 
57.3 

62.0 
66.3 

68.8 

83.8 
107.0 
134.0 
163.0 
197.0 
220.3 

(Berkeley,  Trans.  Roy.  Soc.  1904,  203. 
A,  213.) 

100  g.  H2O  dissolve  26.945  g.  CsNO3  at 
25°.  (Haigh,  J.  Am.  Chem.  Soc.  1912,  34. 
1148.) 

Sp.  gr.  20°/4°  of  a  normal  solution  of  CsNO3 
=  1.140905;  of  a  0.5  normal  solution  = 
1.07001.  (Haigh.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899,  II. 
1014;  Naumann,  B.  1904,  37.  4328.) 

Solubility  in  glycol=8%  at  ord.  temp, 
(de  Coninck,  Belg.  Acad.  Bull.  1905,  359.) 


Caesium  hydrogen  nitrate. 

CsNO3,  HNO3.  Sol.  in  H2O.  (Wells,  Am. 
Ch.  J.  1901,  26.  273.) 

CsNO3,  2HNO3.    (W.) 

Caesium  cerium  nitrate,  Cs2Ce(NO3)6. 

Sol.  in  H2O;  very  si.  sol.  in  HNO3.  (Meyer, 
Z.  anorg.  1901,  27.  371.)  ' 

Sol.  in  HNO3.    (Meyer,  B.  1900,  33.  2137.) 

Caesium  ferric  nitrate,  CsNO3,  Fe(NO3)3+ 
7H2O. 

Deliquescent.  (Wells,  Am.  Ch.  J.  1901, 
26.  276.) 

Caesium  silver  nitrate,  CsNO3,  AgNO3. 

Sol.  in  H2O.  (Russell  and  Maskelyne,  Roy. 
Soc.  Proc.  26.  357.) 

Caesium  thorium  nitrate,  Cs2Th(NO3)6. 

Decomp.  by  H2O;  si.  sol.  in  HNO3.  (Meyer, 
Z.  anorg.  1901,  27.  384.) 

Caesium  uranyl  nitrate,  Cs(UO2)(NO3)3. 

Decomp.  by  H2O.  Sol.  in  cone.  HNO». 
(Meyer,  B.  1903,  36.  4057.) 

Decomp.  by  H2O  at  low  temp.,  so  that  the 
solid  phase  in  contact  with  the  solution  con- 
sists of  the  double  salt  and  CsNO3.  At  16.1° 
100  pts.  by  wt.  of  the  solution  in  H2O  con- 
tain 31.39  pts.  UO2  and  6.59  pts.  Cs.  (Rim- 
bach,  B.  1904,  37.  477.) 

Calcium  nitrate,  basic,  Ca?(NO3)2,  CaO2H2  + 


Decomp.  by  H2O.  (Werner,  A.  ch.  (6)  27. 
570.) 

+H2O.  As  above.  (Rousseau  and  Tite, 
C.  R.  114.  1184.) 

Calcium  nitrate,  Ca(NO3)2. 

Deliquescent.  Very  sol.  in  H2O  with  evolu- 
tion of  much  heat. 

100  pts.  H2O  at  0°  dissolve  84.2  pts. 
Ca(NO3)2.  (Poggiale.) 

100  pts.  H2O  at  0°  dissolve  93.1  pts. 
Ca(NO3)2.  (Mulder.) 

Sol.  in  0.25  pt.  cold  PhO  with  reduction  of  temp. 
Sol.  in  all  proportions  in  boiling  HeO.  (Berzelius.) 

Sol.  in  2  pts.  cold,  and  0.6667  pt.  boiling  HjO. 
(Fourcroy.) 

Sat.  Ca(NOs)2+Aq  at  12.5°  contains  33.8%.  (Has- 
senfratz,  A.  ch.  28.  29.) 

Solubility  in  H2O. 
100  g.  of  the  solution  contain  at: 
55°          80°          90°          100° 
78.16      78.20      78.37      78.43  g.  Ca(NO3)2, 


125C 


147.5° 
78.80 


151°  (bpt.  of  sat.  solution  at 
760  mm.) 
78.57      78.80    79.00  g.  Ca(NO8)2. 

The  anhydrous  salt  is  the  stable  solid  phase 
above  51.3°.  (Bassett  and  Taylor,  Chem. 
Soc.  1912,  101.  580.) 


560 


NITRATE,  CALCIUM 


100  g.  sat.  Ca(NO3)2+Aq  contain  77.3  g 
Ca(NO3)2  at  25°.  (Taylor  and  Henderson. 
J.  Am.  Chem.  Soc.  1915,  37.  1692.) 

See  also  +2,  3,  and  4H2O. 

Sp.gr.  of  Ca(NO3)2+Aq  at  room  temp 
containing : 

17.55        30.10        40.13  %  Ca(NO3)2. 
1.1714       1.2739       1.3857 

(Wagner,  W.  Ann.  1883;  18.  270.) 
Sp.  gr.  of  Ca(NO3)2+Aq  at  17.5 


Ca(NO3)2+Aq  containing  7.15%  Ca(NO3)2 
has  sp.  gr.  20°/20°  =  1.0554. 

Ca(NO3)2+Aq  containing  7.91%  Ca(NO3)2 
has  sp.  gr.  20°/20°  =  1.0613. 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  284.) 

Sp.  gr.  of  Ca(NO3)2+Aq'at  20°  containing 
M  g.  mols.  of  salt  per  liter. 
M  0.0125      0.025        0.05        0.125 

Sp.gr.      1.001846  1.003166  1.00604  1.01523 


Ca(NO3)2 

Sp.  gr. 

Ca(N03)2 

Sp.  gr. 

M             0.25          0.5            0.75 
Sp.  gr.      1.03074     1.06011     1.08874 

M             1.00          1.50 
Sp.  gr.      1.11751     1.17375 
(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38 

Saturated  Ca(NO8)2+Aq  containing 
pts.  Ca(NO3)2  to  100  pts.  H2O  boils  a 
(Legrand);  152°  (Kremers). 
Forms  a  crust  at  141°,  and  contains 
pts.  Ca(NO3)2  to  100  pts.  H2O;  highest 
observed,  151°.    (Gerlach,  Z.  anal.  26.  4 

B.-pt.     of    Ca(NO3)2+Aq    containing 
Ca(NO3)2  to  100  pts.  H2O.    G  =  a 
ing  to  Gerlach  (Z.  anal.  26.  447 
according  to  Legrand  (A.  ch.  (2)  59 

.  704.) 

351.2 
it  151° 

333.5 

temp. 

27.) 

;  pts. 

ccord- 
).  j 

1 
5 
10 
15 
20 
25 
30 

1.009 
1.045 
1.086 
1.129 
1.174 
1.222 
1.272 

35 
40 
45 
50 
55 
60 

1.328 
1.385 
1.447 
1.515 

'1.588 
1.666 

(Franz,  J.  pr.  (2)  5;  274.)    , 
Sp.  gr.  of  Ca(NO3)2+Aq  at  17.5°. 

Ca(N03)2 

Sp.  gr. 

Catf 

?0 
JO  3)  2 

Sp.  gr. 

10 
20 
30 

1.076 
1.163 
1.261 

40 
50 
'    60 

1.368 
1.483 
1.605 

,  L  = 

.436). 

B.-pt 

G 

L 

B.-pt. 

G 

L 

(Gerlach,  Z.  anal.  27.  283.) 
Sp.  gr.  of  Ca(NO3)2+Aq  at  18°. 

101° 
102 
103 
104 
105 
106 
107 
108 
109 
110 
111 
112 
113 
114 
115 
116 
117 
118 
119 
120 
121 
122 
123 
124 
125 
126 

10 
20 
30 
40 
50 
60 
70 
80 
89 
98 
106.5 
114.5 
122.5 
130 
137.5 
144 
150.5 
157 
163.5 
170 
176 
182.5 
189 
195.5 
202 
208.5 

15 
25.3 
34.4 
42.6 
50.4 
57.8 
64.9 
71.8 
78.6 
85.3 
91.9 
98.4 
104.8 
111.2 
117.5 
123.8 
130 
136.1 
142.1 
148.1 

160  !l 
172  '.2 
184  .'5 

127 
128 
129 
130 
131 
132 
133 
134 
135 
136 
137 
138 
139 
140 
141 
142 
143 
144 
145 
146 
147 
148 
149 
150 
151 
151.97 

215.5 
222.5 
230 
237.5 
245 
253 
261.5 
270 
278.5 
287 
296 
305 
314.5 
324 
333.5 
343.5 
354 
364.5 
375 
386 
397.5 
409 
420.5 
432.5 
444.5 
455.68 

197^0 
209!  5 
222^2 
235^1 
248  .1 
261.3 
274  .'7 
288  .'4 
302-6 
317.4 
333^2 

351  .'2 
362.2 

Ca(N03)2 

Sp.  gr.  ' 

Ca(N03)2 

Sp.  gr. 

6 
12 
25 

.25 
.5 
.0 

1.0487 
1.1016 
1.2198 

37 

50 

.5 
.0 

1.3546 
1.5102 

(Kohlrausch,  W.  Ann.  1879.  1 

Sp.  gr.  of  Ca(NO3)2+Aq  at  24.65°. 
of  g.X^>  mol.  wt.  dissolved  in 
H2O;  b=sp.  gr.  if  a  is  Ca(NO3) 
YZ   mol.   wt.  =  118;  c  =  sp.    gr. 
Ca(NO3)2,  y%  mol.  wt.  =82. 

a=no. 
1000  g. 
2,  4H2O, 
if   a   is 

a 

b 

c 

a 

b 

c 

1 

2 
3 
4 
5 

1.056 
1.104 
1.145 
1.181 
1.213 

1.059 
1.112 
1.160 
1.205 
1.246 

6 

7 
8 
9. 
10 

1.243 
1.270 
1.294 
1.316 
1.336 

1.286 
1.323 

(Favre  and  Valson,  C.  R.  79.  968.) 
Sp.  gr.  of  Ca(NO3)2+Aq  at  25°. 

Concentration  of 
Ca(NOs)2+Aq. 

Sp.  gr. 

Sat.  Ca(NO3)2+Aq  boils  at  132°.     (Ord- 
way,  Sill.  Am.  J.  (2)  27.  14.) 

Cone.  HNO3  precipitates  Ca(NO3)2  from 
ts  aqueous  solution.      (Mitscherlich,   Pogg. 
18.  159.) 
Very  sol.  in  cone.   HNO3.     (Rawson,   J. 
Soc.  Chem.  Ind.  1897,  16.  113.) 

1-normal 

l/l       " 

1.0596 
1.0300 
1.0151 
1,0076 

(Wagner,  Z.  phys.  Ch.  1890,  6.  36.) 

NITRATE,  CALCIUM 


561 


Solubility  in  HNO3+Aq  at  25°. 

Solubility  of  Ca(NO8)2+CaS2O8  at  t°. 

100  g.  of  the  solution  contain 

Solid  phase 

t° 

Ca(Nbs)2 

m 

CaS203 

Solid  phase 

G.  Ca(NOs)2 

G.  HNOs 

57.98 
54.82 
52  96 

0.00 

3.33 

5.87 

1 

9 

46.02 
45.68 
27.92 

5.46 
6.81 
10.46 

Ca(N03)2,  4H20 
"    CaS2O8,  6H2O 
CaS2O3,  6H2O 

51  .'58 

7.21 

10.49 

22.81 

u 

47.82 

11.27 

29.33 

45.59 
40.70 

13.71 
19.65 

Ca(NO3)2+4H2O 

25 

54.03 

4.27 

Ca(N03)2>  4H20 

38.17 
34.46 
32.84 

22.80 

28.81 
32.63 

"••;•' 

50.25 
45.92 
42.93 

9.10 
13. 
13.83 

"+CaS2O8,  6H2O 
CaS2O3,  6H2O 

32.50 

33.52 

32.01 

17.09 

(( 

33.44 

35  63 

' 

19.51 

23.78 

29.05 

41'.  66 

Ca(N08)2+3H2O 

8.15 

29.85 

it 

27.79 

45.70 

31.09 

40.56 

(Kremann  and  Rothmund,  Z.  anorg.  1914, 

26.07 

45.70 

86.  373.) 

17.41 
12.25 

55.48 
62.05 

Ca(N03)2+2H20 

9.34 

65.69 

8.52 
5.06 

67.20 
71.12 

Very  easily  sol.  in  liquid  NH8.    (Franklin, 
Am.  Ch.  J.  1898,  20.  827.) 

2.53 

74.77 

Sol.  in  0.8  pt.  alcohol  (Macquer);  1  pt. 

1.05 
0.54 

78.56 
80.83 

•  Ca(NO3)2 

boiling  alcohol.    (Bergmann.) 
Dry  Ca(NO3)2  is  sol.  in  7  pts.  alcohol  at 

0.36 
0.01  (about) 

85.83 
90.90 

15°  and  1  pt.  boiling  alcohol.    (Bergmann.) 

0.00 

96.86 

These  results  show  that  the  hydrates  of 
Ca(NO3)2  which  are  stable  at  25°  in  contact 

Sp.  gr.  of  Ca(NO8)2+alcohol. 

with     HNO3+Aq     are     Ca(NO3)2+4H2O, 
+3H2O  and  +2H2O. 

%  Ca(NOs)2                          Sp.  gr.  20°/20° 

(Bassett  and  Taylor,  Chem.  Soc.  1912,  101. 

0                                      0.7949 

582.) 

4.96                                 0.8278 

6.47                                  0.8383 

Sol.  in  glacial  HC2H3O2.    (Persoz.) 

Sol.  in  sat.  KNO3+Aq  with  elevation  of 

temp,    and   pptn.    of   a   portion   of   KNO3. 

(Fourcroy  and  Vauquelin,  A.  ch.  11.  135.) 

Solubility  of  Ca(NO3)2+NaN08  at  t°. 


t° 

% 

Ca(NOi)a 

% 

NaNOa 

Solid  phase 

9 

47.51 
46.08 
26.67 
11.76 

9.51 
12.56 
23.32 
34.26 

Ca(N08)2,  4H20 
"  +NaNO8 

NaNO3 
t( 

25 

54.58 
53.22 
52.73 
52.40 
37.31 
26.91 
14.61 

7.25 
10.70 
12.08 
11.58 
19.48 
24.98 
36.12 

Ca(NO3)2,  4H2O 
(t 

"  +NaNO8 

NaNO8 
u 

n 
<t 

(Kremann  and  Rothmund,  Z.  anorg.  1914, 
86.  373.) 


(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  284.) 


Solubility  in  ethyl  alcohol  -f-Aq  at  25°. 


%  C2H5OH  in 
the  solvent 

%  CzEUOH  in 
the  solution 

%  Ca(NO3)2in 
the  solution 

*o 

0 

82.5 

*25.1 

5.8 

77.0 

*50.1 

15.2 

69.52 

*60.1 

20.4 

66.08 

*63.9 

22.4 

64.94 

70.4 

'26.5 

62.3 

72.0 

27.39 

61.96 

73.4 

28.5 

61.15 

75.3 

29.9 

60.3 

*84.9 

35.9 

57.7 

*99.1 

48.1 

51.4 

*  Metastable  solutions. 
(D'Ans  and  Siegler,  Z.  phys.  Ch.  1913,  82.  43.) 


562 


NITRATE,  CALCIUM 


Solubility  of  Ca(NO3)2.  2C2H5OH  in  C2H5OH 

Solubility  in  H2O  at  t°. 

+Aq  at  25°. 

100  g.  of  the  solution 

contain  g.  Ca(NO3 

%  C2H5OH  in       %  C2H5OH  in       %  Ca(NO3)2  in 

at  t°. 

the  solvent             the  solution             the  solution 

t° 

•      G.  Ca(NO3)2 

98  .  1                   60  .  2                  38  .  6 

94!l                   54^6                  41.9 

—26.7 

43.37 

85.8                  42.5                  50.97 

—10.0 

47.31 

80.5                  35.8                  55.3 

0.0 

50.50 

75.3                  29.9                  60.28 

+5.0 

-i  r\    A 

51.97 

CO      CC 

(D'Ans  and  Siegler,  I.  c.) 

10.0 
15.0 

5o.55 
54.94 

See  also  under  +4H20. 

20.0 

56.39 

25.0 

57.98 

30.0 

60.41 

Solubility  in  organic  solvents. 

35.0 

A  C\     A 

62.88 

Solvent                          %  Ca(NO3)2  in  the 
solution  at  25° 

40.0 
42.4 

68^68 

42.  £ 

> 

68.74 

Methyl  alcohol                       65.5 
Ethyl  alcohol                          52.0 

42.7 
42.45 

mpt.  of  Ca(NO3)2+4H2< 
71.70 

Propyl  alcohol                        36  .  5 

Isobutyl  alcohol                     25  .  0 

(Bassett  and 

Taylor,  I.  c.) 

Amyl  alcohol                           13.3 

Acetone                                   58  .  5 

(D'Ans  and  Siegler,  I.  c.) 

Solubility  of  a  and  ft  modifications  in  H2 
at  t°. 

a  modification  is  the  stable  form. 

Sol.    in    1.87    pts.    ether-alcohol    (1  :  1). 

(Fresenius,  Z.  anal.  32.  191.) 

r  c  CNO  }•» 

Ether  ppts.  Ca(NO3)2  from  its  alcoholic 

t° 

in  100  g.  of" 

Solid  phase 

solution.    Easily  sol.  in  boiling  amyl  alcohol. 

/T~>                      "                Cl'11         A                 T      H  Aft        r-O    \ 

solution 

(Browning,  bill.  Am.  J.  143.  53.) 
Sol.  in  acetone.     (Naumann.  B.  1904.  37. 

0 

50.17 

aCa(NO3)2+4H2( 

4328.) 

22.2 

56.88 

a                  " 

Insol.  in  benzonitrile.    (Naumann,  B.  1914, 

25.0 

57.90 

a 

47.  1370.) 

30.0 

60.16 

a 

Insol.  in  methylal.    (Eidmann,  C.  C.  1899. 

30.0 

61.57 

ft 

II.  1014.) 

34.0 

63.66 

ft 

1  g.  Ca(NO3)2  is  sol.  in  1.44  g.  methyl 

35.0 

62.88 

a                   ' 

acetate  at  18°.    Sp.  gr.  18°/4°  of  sat.  solution 

38.0 

64.34 

a                    ' 

a                              it 

=  1.313.    (Naumann,  B.  1909,  42.  3795.) 

38.0 

66.65 

ft 

Sol.  in  ethyl  acetate.    (Naumann,  B.  1910,, 
43.  314.) 

39.0 
139.6 

67.93 
69.50 

ft 
ft 

+2H2O.    Solubility  in  H2O. 

239.0 

75.34 

ft 

100  g.  of  the  solution  contain  at: 

40.0 

66.21 

a 

49°            51° 

1-42.7 

69.50 

a                    " 

77.49        78.05  g.  Ca(NO3)2. 

242.4 

71.70 

a                   " 

Solutions  in  stable  equilibrium  with  the 
dihydrate  can  only  exist  between  the  limits 
of  temp.  48.4°  and  51.3°.    (Bassett  and  Tay- 

1 mpt.  of  hydrate. 
2  reflex  pt. 

lor,  Chem.  Soc.  1912,  101.  580.) 
+3H2O.    Solubility  in  H2O. 
100  g.  of  the  solution  contain  at: 

(Taylor  and 

Henderson, 
1915,  37. 

J.  Am.  Chem.  So( 
1692. 

40°         45°         50°       '  51° 

70.37      71.45      73.79      74.73  g.  Ca(NO3)2. 
Mpt.  of  Ca(NO3)2+3H2O=51.1°. 
(Bassett  and  Taylor,  I.  c.) 

Sp.  gr.  of  solution  sat.  at  18°  =  1.548,  con 
taining  54.8%  Ca(NO3)2.     (Mylius,  B.  1897 
30.  1718.) 

+4H2O.  Ca(NO3)2+4H2O  melts  in  its 
crystal  H2O  at  44°.  (Tilden,  Chem.  Soc.  45. 
409.) 


NITRATE,  CERIC  ZINC 


563 


Solubility  in  ethyl  alcohol  +Aq  at  25°. 

Ceric  magnesium  nitrate,  CeMg(NO3)6. 
IQTT  n 

%  C2H5OH  in 
the  solvent 

%  C2H5OH  in 
the  solution 

%  Ca(NO3)2in 
the  solution 

-|-orl2\J. 

Decomp.  by  H2O;  sol.  in  HNO3+Aq  with- 

out decomp.     (Meyer,  Z.  anorg.   1901,  27. 

0 

0 

57.5 

373.) 

18.3 

3.5 

56.1 

39.2 

8.1 

55.2 

Cerous   manganous   nitrate,   2Ce(NO3)3, 

59.2 

14.1 

52.9 

3Mn(NO3)2+24H2O. 

80.4 

22.3 

50.2 

Sol.  in  H2O.    (Lange,  J.  pr.  82.  129.) 

90.4 

29.4 

49.0 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 

99.4 

31.1 

49.7 

1.325)  contains  193.1  g.  hydrous  salt  at  16°. 

99.4 

31.2 

52.0 

(Jantsch.)     • 

99.4 

29.5 

56.2 

60.1 

28.3 

58.9 

Ceric    manganous    nitrate,    CeMn(NO3)6-f- 

60.1 

27.8 

60.0 

8H20. 

60.1 
60.1 

27.3 
26.5 

60.7 
62.3 

Decomp.  by  H2O  and  dil.  HNO3;  sol.  in 
cone.  HNO3  without  decomp.     (Meyer,  Z. 

(D'Ans  and  Siegler,  Z.  phys.  Ch.  1913,  82.  42.) 

anorg.  1901,  27.  377.) 

Calcium  nitrate  hydrazine,  Ca(NO3)2,  2N2H4 

+H20. 
Ppt.    (Franzen,  Z.  anorg.  1908,  60.  288.) 

Calcium  nitrate  tungstosilicate,  Ca2Wi2SiO4o, 

Ca(NO3)2. 

+  13H2O  and  +15H2O.  Decomp.  by  H2O. 
(Wyrouboff,  Chem.  Soc.  1897,  72.  (2)  176.) 

Cerous  nitrate,  Ce(NO3)3+6H2O. 

Not  very  deliquescent.    (Jolin.) 

Very  sol.  in  H2O;  sol.  in  2  pts.  alcohol. 
(Vauquelin.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899.  II. 
1014;  Naumann,  B.  1904,  37.  4328.) 

Ceric  nitrate,  Ce(NO3)4. 

Deliquescent.  Decomp.  by  hot  H2O. 
(Berzelius.) 

Sol.  in  alcohol.    (Dumas.) 

Basic  compounds  containing  12  mols.  or 
less  CeO2  to  1  mol.  N^Os  may  be  obtained, 
which  are  sol.  in  H2O.  (Ordway.) 

Cerous  cobaltous  nitrate,  2Ce(NO3)3, 
3Co(NO3)2+24H2O. 

Deliquescent.  Easily  forms  supersaturated 
solutions.  (Lange,  J.  pr.  82.  129.) 

1  1.  sat.  solution  in  HN08+Aq  (sp.  gr. 
1.325)  contains  103.3  g.  hydrous  salt  at 
16°.  (Jantsch,  Z.  anorg.  1912,  76.  321.) 

Ceric  cobaltous  nitrate,  CeCo(NO3)6-|-8H2O. 
Decomp.  by  H2O  when  heated;  sol.  in  cold 
H2O;  si.  sol.  in  HNO3.     (Meyer,  Z.  anorg. 
1901,  27.  376.) 

Cerous   magnesium   nitrate,    2Ce(NO3)3, 
3Mg(NO3)2+24H2O. 

Slightly  deliquescent.  Easily  sol.  in  H2O 
or  alcohol,  and  easily  forms  supersaturated 
solutions.  (Holzmann,  J.  pr.  75.  330.) 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  63.8  g.  hydrous  salt  at  16°. 
(Jantsch,  Z.  anorg.  1912,  76.  321.) 


Cerous  nickel  nitrate,  2Ce(NO3)3,  3Ni(NO3)2 
+24H2O. 

Easily  sol.  in  H2O.  (Holzmann,  J.  pr.  76. 
321.) 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  80.3  g.  hydrous  salt  at  16°. 
(Jantsch.) 

Ceric  nickel  nitrate,  CeNi(N03)6+8H2O. 

Decomp.  by  H2O  when  heated;  sol.  in  H2O 
in  the  cold;  si.  sol.  in  HNO3.  (Meyer,  Z. 
anorg.  1901,  27.  375.) 

Cerous  potassium  nitrate,  Ce(NO3)3,  2KN03 

+2H20. 
Sol.  in  H20.    (Lange,  J.  pr.  82.  136.) 

Ceric  potassium  nitrate,  CeK2(NO3)6. 

Sol.  in  H20  with  decomp.  (Meyer,  Z. 
anorg.  1901,  27.  370.) 

Efflorescent.     (Holzmann,  J. 
pr.  75.  324.) 

Ceric  rubidium  nitrate,  CeRu2(NO3)6. 
Very  sol.  in  H2O  ;  si.  sol.  in  HNO3.    (Meyer.) 

Ceric  sodium  nitrate. 
Deliuescent. 


tion 


•eliquescent.     Decomp.  by  recrystalliza- 
..    (Holzmann.) 

Cerous    thallous    nitrate,     [Ce(NO3)5]Tl2-{- 

4H20. 

Very  hydroscopic.  Decomp.  by  H2O. 
(Jantsch,  Z.  anorg.  1911,  69.  229.) 

Cerous  zinc  nitrate,  2Ce(NO3)3,  3Zn(NO3)2-f 
24H2O. 

Sol.  in  H2O.  Easily  forms  supersat.  solu- 
tions. (Lange,  J.  pr.  82.  129.) 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
]  325)  contains  124.1  g.  hydrous  salt  at  16°. 
(Jantsch,  Z.  anorg.  1912,  76.  321.) 

Ceric  zinc  nitrate,  ZnCe(NO3)6+8H20. 

Decomp.  by  H2O;  sol.  in  HN03+Aq. 
(Meyer,  Z.  anorg.  1901,  27.  374.) 


564 


NITRATE,  CEROCERIC  ZINC 


Ceroceric    zinc    nitrate    (?),    Ce3O4,    2ZnO, 

6N2O5+18H2O  (?). 

Easily  sol.  in  H2O.  (Holzmann,  J.  pr.  76. 
321.) 

Chromic  nitrate,  basic,  Cr2O(NO3)4. 
Sol.inH2O.    (Lowel.) 
+12H2O.    Sol.  in  H2O.    (Ordway.) 

Chromic  nitrate,  Cr(NQ3)3+9H2O. 

Very  sol.  in  H2O  and  alcohol.    (Lowel.) 

Melts  in  its  crystal  H2O  at  36.5°.  Sat. 
Cr(NO3)3+Aq  boils  at  125.6°.  (Ordway.) 

Sp.  gr.  of  Cr(NO3)3-f-Aq. 

M  =  concentration  of  solution  in  gram, 
mols. 

W  =  wt.  of  25  cc.  of  solution. 
M    0.0934    0.1868    0.3736    0.5604    0.9340 
W  25.4300  25.8828  26.7302  27.5524  29.3072 

M     1.1208     1.3076     1.4944     1.8680 
W  30.0668  30.8464  31.6327  33.3379 
(Jones  and  Getman,  Z.  phys.  Ch.  1904,  49. 
426.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328;  Eidmann,  C.  C.  1899,  II.  1014.) 

Chromic  nitrate  chloride,  CrCl2(NO3). 

Sol.  in  H2O  and  alcohol.  (SchinyA.  124. 
177.) 

Cr(NO3)2Cl.    (Schiff.) 

Chromic  nitrate  sulphate,  Cr2(S04)(NO3)4. 

Hygroscopic.    Completely  sol.  in  H2O. 

Cr2(S04)2(N03)2.  Sol.  inH20.  (Schiff,  A. 
124.  174.) 

Cobaltous  nitrate,  basic,  6CoO,  N2O5+5H2O. 

Ppt.  Gradually  sol.  in  H2O  with  deposition 
of  CoO.  (Winkelblech,  A.  13.  155.) 

Sol.  in  cold  HC1,  and  HNO3+Aq.  De- 
comp.  by  hot  KOH+Aq. 

4CoO,  N2O6+6H2O.  Ppt.  (Habermann, 
M.  6.  432.) 

Cobaltous  nitrate,  Co(NO3)2. 

Deliquescent  in  moist  air.  Very  sol.  in 
H20. 

See  +3,  6,  and  9H2O. 

Sp.  gr.  of  aqueous  solution  at  17.5°  con- 
taining: 

5  10  15  20%Co(NO3)2, 

1.0462      1.0906      1.1378      1.1936 

25  30  35  40%Co(NO3)2. 

1.2538      1.3190      1.3896      1.4662 

Sp.  gr.  of  sat.  solution  =  1.5382. 
(Franz,  J.  pr.  (2)  6.274.) 

Sp.  gr.  of  Co(NO3)2+'Aq  at  room  temp, 
containing: 

8.28         15.96      24.528%  Co(NO3)2. 
1.0732      1.1436      1.2288 

(Wagner,  W.  Ann.  1883,  18.  268.) 


Sp.  gr.  of  Co(NO3)2+Aq  at  25C 


Concentration  of 

Co(NCh)2+Aq. 


1-normal 

r-       " 


V4- 


Sp.  gr. 


1.0728 
1.0369 
1.0184 
1.0094 


(Wagner,  Z.  phys.  Ch.  1890,  5.  37.) 

Sp.  gr.  at  20°  of  Co(NO3)2+Aq  containing 
M  g.  mols.  Co(NO3)2  per  liter. 
M         0.01          0.025        0.05          0.075 
Sp.  gr.  1.001496  1.003863  1.007579  1.011289 

M         0.10          0.25          0.5  0.75 

Sp.  gr.  1.015084  1.03737     1.07415     1.11204 

M         1.0  1.5  2.0 

Sp.  gr.  1.14612     1.21720     1.28576 

(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38.  715.) 

Sol.  in  liquid  NH3.     (Guntz,   Bull.   Soc. 
1909  (4)  6.  1009.) 

100  g.  sat.  solution  in  glycol  contains  80  g. 
Co(NO3)2.    (de  Coninck,  C.  C.  1905,  II.  883.) 

Sol.  in  ethyl  acetate.    (Naumann,  B.  1904, 
37.  3601.) 

+3H2O.    Solubility  in  H2O. 

Sat.  solution  contains  at: 
55°      62°      70°      84°      91°  mpt. 
61.74  62.88  64.89  68.84  77.21%  Co(NO,)2. 

(Funk,  Z.  anorg.  1899,  20.  408.) 

+6H2O.    Melts  in  its  crystal  H2O  at  56° 
(Ordway);  38°  (Tilden). 
Solubility  in  H2O. 
Sat.  solution  contains  at: 
—21°    —10°     —4°       0° 
41.55    43.69    44.85     45.66%  Co(NO3)2, 


+18C 
49.73 


41°        56°  mpt. 
55.96     62.88%  Co(NO3)2. 

(Funk,  Z.  anorg.  1899,  20.  408.) 


Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  827.) 

Easily  sol.  in  alcohol.  Sol.  in  1  pt.  strong 
alcohol  at  12.5°.  (Wenzel.) 

Easily  sol.  in  acetone.  (Krug  and  M'Elroy, 
J.  Anal.  Ch.  6.  184.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Difficultly  sol.  in  ethyl  acetate.  (Nau- 
mann, B.  1910,  43.  314.) 

+9H2O.    Solubility  in  H2O. 

Sat.  solution  contains  at: 

—26°      —23.5°      —20.5° 

39.45  40.40          42.77%  Co(N03)2. 

Cryohydrate  is  formed  at  — 29°.  (Funk, 
Z.  anorg.  1899,  20.  409.) 


NITRATE,  CUPRIC 


565 


Cobaltous     didymium    nitrate,     3Co(NO3)2, 

2Di(NO3)3-j-48H2O. 

Very  deliquescent.  (Frerichs  and  Smith, 
A.  191.  331.) 

Cobaltous    gadolinium    nitrate,    3Co(NO3)2, 

2Gd(NO3)3+24H2O. 

1  1.  sat.  solution  in  HNO3  (sp.  gr.  1.325) 
contains  451.4  g.  hydrous  salt  at  16°. 
(Jantsch,  Z.  anorg.  1912,  76.  303.) 

Cobaltous    lanthanum    nitrate,    3Co(NO3)2, 

2La(NO3)3+24H20. 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  109.2  g.. hydrous  salt  at  16°. 
(Jantsch,  Z.  anorg.  1912,  76.  303.) 


Cobaltous   neodymium   nitrate,   3Co(NO3)2, 
2Na(NO3)3+24H20. 

5 
1.0452 

10 

1.0942 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  151.6  hydrous  salt  at  16°. 

20 
1.2036 

25 
1.2644 

(Jantsch.) 

35 

40 

f^rkHflltrtnc  nrac*»rkflvtriiitin  riifrato    3f^r»f''\rO..'W 

1.3974 

1.4724 

2Pr(N03)3+24H2O. 
1  1.  sat.  solution  in  HN03+Aq  (sp.  gr. 


8H2O. 

Hydroscopic;  sol.  in  HNO3+Aq.  (Meyer, 
Z.  anorg.  1901,  27.  387.) 

Cobaltous  nitrate  ammonia,  Co(NO3)2,  6NH3 
+2H2O. 

Decomp.  by  H2O  with  separation  of  basic 
nitrate.  (Fremy.) 

Sol.  in  NH4OH+Aq.    (Hess.) 

Cobaltous   nitrate   cupric   oxide,   Co(NO3)2, 

3CuO+3H2O. 
Ppt.    (Mailhe,  C.  R.  1902,  134.  234.) 

Cobaltous  nitrate  hydrazine,   Co(NO3)2, 

3N2H4. 

Decomp.  by  hot  H2O.  (Franzen,  Z.  anorg, 
1908,  60.  274.) 

Cupric  nitrate,  basic,  2CuO,  N2O5. 

(Ditte,  A.  ch.  1879,  (5)  18.  339.) 

4CuO,  N295+3H2O.  Insol.  in  H2O.  Eas- 
ily sol.  in  acids.  (Graham,  A.  29.  13.) 

Insol.  in  H2O;  easily  sol.  in  acids.  (Athan- 
asesco,  Bull.  Soc.  1895,  (3)  11.  1113.) 

+3^H2O.  Insol.  in  H2O,  and  decomp.  by 
heat.  (Casselman,  Z.  anal.  4.  24.) 


Cupric  nitrate,  Cu(NO3)2. 

Deliquescent.  Very  easily  sol.  in  H2O  or 
alcohol;  also  in  moderately  cone.  HNO3+Aq, 
but  is  precipitated  from  cone,  aqueous  solu- 
tion by  HNO3-f  Aq  of  1.522  sp.  gr.  (Mit- 
scherlich,  Pogg.  18.  159.) . 

Sat.  Cu(NO3)2+Aq  contains  at: 
—10°        —3°         +3° 
38.8  41.6         44.5%  Cu(NO3)2, 

8°  20°          32° 

48.5          54.1    %     61.2%  Cu(N"O3)2. 

(fitard,  A.  ch.'  1894,  (7)  2.  528.) 
See  +3,  6,  and  9H2O. 

Sp.  gr.  of  Cu(NO3)2-hAq  at  17.5°  contain- 
ing: 

15%  anhydrous  salt, 
1.1442 

30%  anhydrous  salt, 
1.3298 

45%  anhydrous  salt. 
1.5576 
(B.  Franz,  J.  pr.  (2)  5.  274.) 

Sp.  gr.  of  Cu(NO3)2-f  Aq  at  15°. 


(Jantsch.) 

%  Cu(N03)2 

Sp.  gr. 

Cobaltous    samarium    nitrate,     3Co(NO3)2, 

5.22 

1.046 

2Sm(N03)3+24H20. 

10.44 

1.094 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  34.27  g.  hydrous  salt  at  16°. 

15.67 
20.85 

1.146 
1.202 

(Jantsch.) 

26.12 

1.262 

/~W»a1frtliei        +Vi/~»tMiirvi        ni+i-a+a          P'/iTl-i  (  XTT^  -^  -  _l_ 

35.00 

1.377 

(Long,  W.  Ann.  1880,  11.  39.) 

Sp.  gr.  of  Cu(NO3)2+Aq  at  room  temp, 
containing: 

18.99        26.68        46.71%  Cu(NO3)2. 
1.1774      1.2637       1.5363 

(Wagner,  W.  Ann.  1883,  18.  272.) 

Sp.  gr.  of  Cu(NO3)2+Aq  at  25°. 


Concentration  of 
Cu(NOi)«+Aq 

Sp.  gr. 

1-normal 

Vr-       " 

V«-     " 

Vs-       " 

1.0755 
1.0372 
1.0185 
1.0092 

(Wagner,  Z.  phys.  Ch. 

Sp.gr.  of  Cu(NO3)2+Aq 
%  Cu(NO3)2      1             5 

1890,  5.  38.) 

at  12.5°. 
10 

14 

Sp.  gr. 


1.0059     1.0320     1.0655     1.0916 


%Cu(NO3)2    20  24  30  34 

Sp.gr.  1.1350     1.1716     1.2320     1.2712 

%Cu(N03)2     40  44  50  56 

Sp.gr.  1.3320     1.3749     1.4440     1.5205 

(Hassenfratz,  Muspratt,  1893,  4.  2243.) 


566 


NITRATE,  CUPRIC,  AMMONIA 


Sp.  gr.  at  20°  of  Cu(NO3)2+Aq  containing 
M  g.  mols.  salt  per  liter. 
M         0.01          0.025        0.05          0.075 
Sp.  gr.  1.001504  1.004076  1.007859  1.011715 

M         0.25  0.50          0.75          0.935 

Sp.  gr.  1.040290     1.07723     1.11469     1.14262 


Sp.  gr.  1.5 


2.0 
1.29262 


M         1.22618 

(Jones  and  Pearce,  Am.  Ch.  J.  1917,  38.  719.) 

Sat.  Cu(NO3)2+Aq  tfoils  at  about  173°. 
(Griffiths.) 

Insol.  in  fuming  HNO3.  (Ditte,  A.  ch. 
1879  (5)  18.  339.) 

Solubility  of  Cu(NO3)2+Pb(NO3)2  in  H2O 
at  20°. 


In  1  1.  of  solution 

Sp.  gr. 

Cu(NOs)2 

Pb(NO3)2 

Solid  phase 

g- 

g.  mol. 

g. 

g.  mol. 

1.354 

70.5 

0.375 

359.5 

1.086 

Pb(N03)2 

1.322 

139.2 

0.742 

257.2 

0.777 

1.321 

226.5 

1.207 

175.1 

0.529 

1.343 

301.8 

1.608 

133.4 

0.403 

1.360 

341.8 

1.821 

117.8 

0.356 

1.451 

519.4 

2.767 

70.5 

0.213 

1.546 

681.7 

3.632 

44.0 

0.133 

1.622 

798.1 

4.252 

28.1 

0.085 

1.700 

943.2 

5.028 

17.2 

0.052 

Pb(NOs)2  + 

Cu(NO3)2.6H2O 

(Fedotieff,  Z.  anorg.  1911,  73.  178.) 

Very  sol.  in  liquid  NH3    (Guntz,  Bull.  Soc. 

1909,  (4)  5.  1007.) 

Easily  sol.  in  liquid  NH3.  (Franklin,  Am. 
Ch.  J.  1898,  20.  827.) 

Insol.  in  liquid  HF.  (Franklin,  Z.  anorg. 
1905,  46.  2.) 

Insol.   in   ethyl   acetate.      (Naumann,   B. 

1910,  43.  314.) 

SI.  sol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1369.) 

+3H2O.  Melts  in  crystal  H2O  at  114.5°. 
(Ordway;  Tilden,  Chem.  Soc.  45.  409.) 

Solubility  in  H2O. 

Sat.  solution  contains  at: 
25°          30°          40°          50° 
60.01       60.44       61.51       62.62%  Cu(NO3)2, 

60°          70°          80°         114.5°  Mpt. 
64.17       65.79       67.51        77.59%  Cu(NO3)2. 
(Funk,  Z.  anorg.  1899,  20.  413.) 

100  pts.  HNO3  dissolve  2  pts.  at  13°,  con- 
siderably more  on  heating.  (Ditte,  A.  ch. 
1879,  (5)  18.  339.) 

Sol.  in  1  pt.  strong  alcohol  at  12.5°.  (Wen- 
zel.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

+6H2O.  Efflorescent.  Melts  in  crystal 
H2Oat38°.  (Ordway.) 


Solubility  in  H2O. 

Sat.  solution  contains  at: 
—21°      —10°         0°          +10° 
39.52       42.08       45.00       48.79%  Cu(NO3)2, 

18°          20°        26.4°  mpt. 
53.86      55.58      63.39%  Cu(NO3)2. 
(Funk,  Z.  anorg.  1899,  20.  413.) 

Sat.  solution  of  Cu(NO3)2+6H2O  in  H2O 
at  20°  contains  5.04  g.  mol.  per  1.  Sp.  gr.  of 
sat.  solution  =  1.688.  (Fedotieff,  Z.  anorg. 
1911,  73.  78.) 

Sat.  solution  of  Cu(NO3)2+6H2O  m{H20 
contains  45.0  g.  Cu(NO3)2  in  100  g.  solution 
at  0°;  53.9  g.  at  18°.  (Mylius,  Z.  anorg.  1912, 
74.411.) 

+9H2O. 

Solubility  in  H2O. 

Sat.  solution  contains  at: 
—23°  —21°  —20° 
36.08  37.38  40.92%  Cu(NO3)2. 

Cryohydrate  is  formed  at  — 24°.  (Funk, 
Z.  anorg.  1899,  20.  414. 


Cupric  nitrate  ammonia  (Cuprammonium 
nitrate),  Cu(NO3)2,  4NH3. 

Easily  sol.  in  H2O,  from  which  it  can  be 
recrystallized.  Sol.  in  alcohol.  (Berzelius.) 

Sol.  in  1  pt.  liquid  NH3.  (Horn,  Am.  Ch. 
J.  1908,  39.  216.) 

Cu(NO3)2,  5NH3.  (Horn,  Am.  Ch.  J. 
1907,  37.  620.) 

4Cu(NO3)2,  23NH3.    (Horn.) 

Cupric  nitrate  hydrazine,  Cu(NO3)2,  N2H4. 

Decomp.  by  H2O.  (Hofmann  and  Marburg, 
A.  1899,  305.  221.) 

Cupric    nitrate    mercuric    oxide,    Cu(NO3)2, 

HgO+3H2O. 

Sol.  in  HC1,  HNO3  and  H2SO4.  (Finzi, 
Gazz.  ch.  it.  1913,  43.  (2)  709.) 

Didymium  nitrate,  basic,  4Di2O3,  3N2O5  + 
15H2O. 

Insol.  in  H2O.    (Marignac.) 

2Di2O3,  3N2O5.  (Becquerel,  A.  ch.  (6)  14. 
257.) 

Didymium  nitrate,  Di(NO3)3. 

Anhydrous.  Very  sol.  in  H2O.  As  sol.  in 
96%  alcohol  as  in  H2O,  and  the  solution  is  not 
precipitated  by  much  ether.  Insol.  in  pure 
ether.  (Marignac,  A.  ch.  (3)  36.  161.) 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  827.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328;  Eidmann,  C.  C.  1899,  II.  1014.) 

+6H2O.  Very  deliquescent.  (Cleve,  Bull. 
Soc.  (2)  43.  361.) 


NITRATE,  IRON 


567 


Didymium  nickel  nitrate,  2Di(NO3)3, 
3M(NO3)2+36H2O. 

Very  deliquescent.  (Frerichs  and  Smith, 
A.  191.  355.) 

See  Neodymium  and  praseodymium. 

Didymium  zinc  nitrate,  2Di(NO3)3,  3Zn(NO3)2 

+69H20. 

Very  deliquescent.    (F.  and  S.) 
-See  Neodymium  and  praseodymium. 

Dysprosium  nitrate,  Dy(NO3)+5H2O. 

Very  sol.  in  H2O;  less  sol.  in  H2O+HNO3. 
Sol.  in  alcohol.  (Urbain,  C.  R.  1908,  146. 
129.) 

Erbium  nitrate,  basic,  2Er2O3,  3N2O6+9H2O. 

Decomp.  by  H2O.  SI.  sol.  in  HNO3. 
(Bahr  and  Bunsen.)  • 

3Er2O3,  4N2O5+20H2O.  (Cleve,  BuU. 
Soc.  (2)  21.  344.) 

Erbium  nitrate,  Er(NO3)3+6H2O, 

Easily   sol.   in   H2O,    alcohol,    and   ether. 

(Hoglund.) 
Sol.  in  acetone.     (Naumann,  B.  1904,  37. 

4328.) 

Gadolinium  nitrate,  Gd(NO3)3+6^H2O. 

Sol.  in  H2O.  (Benedicks,  Z.  anorg.  1900, 
22.  406.) 

+5H2O.    Sol.  inHNO3.    (B.) 

Gadolinium  magnesium  nitrate,  2Gd(NO3)3, 

3Mg(NO3)2+24H2O. 
1  1.  sat.  solution  in  HNO3+Aq  (sp. 
1.325)  contains  352.3  g.  hydrous  salt  at  1 


(Jantsch,  Z.  anorg.  1912,  76.  303.) 


y 
,  76. 


gr. 
6°. 


Gadolinium      nickel      nitrate,     2Gd(NO3)3, 

3Ni(NO3)2+24H2O. 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  400.8  g.  hydrous  salt  at  16°. 
(Jantsch.) 

Gadolinium       zinc       nitrate,      2Gd(NO3)3, 

3Zn(NO3)2+24H2O. 

1  1.  sat.  solution  in  HN03+Aq  (sp.  gr. 
1.325)  contains  472.7  g.  hydrous  salt  at  16°. 

(Jantsch.) 

Gallium  nitrate,  Ga(NO3)3. 
Very  deliquescent,  and  sol.  in  H2O.  (Dupre*.) 

Glucinum  nitrate,  basic,  2G1O,  N2O6+ 
3H2O  (?). 

Sol.  in  H2O. 

3G1O,  N2O5.  Sol.  in  H20.  (Ordway,  Sill. 
Am.  J.  (2)  26.  205.) 

Compounds  more  basic  than  this  are  insol. 
in  H2O.  (Ordway.) 


Glucinum  nitrate,  G1(N03)2+3H2O. 

Very  deliquescent.  (Joy,  Sill.  Am.  J.  (2) 
36.  90.) 

Easily  sol.  in  H2O  and  alcohol.  (Vauquelin.) 

Melts  in  its  crystal  H2O  at  29.4°.  (Ord- 
way.) 

Sat.  Gl(NO3)2+Aq  boils  at  140.5°.  (Ord- 
way.) 

Gold  (auric)  nitrate,  basic,  Au2O3,  N2O6-J- 
2/5H2O,   or  Auryl  nitrate,  (AuO)NO3+ 


(Schottlander,  A.  217.  364.) 

2Au2O3,     N2O5+2H2O  =  Au4O5(NO3)2-f- 
2H2O.     Slowly  sol.  in  HNO3+Aq  at  100°. 
(Schottlander,  A.  217.  356.) 

Gold  (auric)  nitrate,  Au(NO3)3+zH2O. 

Decomp.  by  H2O.  Sol.  in  acetone.  (Han- 
riot  and  Raoult,  C.  R.  1912,  155.  1086.) 

Gold    (auric)   hydrogen   nitrate,   Au(NO3)3r 

HNO3+3H2O. 

Decomp.  by  H2O.  Sol.  in  HNO3+Aq. 
(Schottlander,  A.  217.  356.) 

Gold  (auric)  potassium  nitrate,  KAu(NO3)4. 

Easily  sol.  in  H2O. 

HK2Au(NO3)6.  Decomp.  immediately  by 
H20. 

2KAu(NO3)4,  K2HAu(NO3)6.  (Schott- 
lander, J.  B.  1884.  453.) 

Gold  (auric)  rubidium  nitrate,  RbAu(NO3)4. 

Easily  sol.  in  H2O. 

HRb2Au(NO3)6.  As  above.  (Schott- 
lander.) 

Gold  (auric)  thallium  nitrate,  TlAu(NO3)4. 

Easily  sol.  in  H2O. 

6Au2O3,  2T12O3,  3N205-fl5H2O.  Ppt. 
(Schottlander.) 

Indium  nitrate,  In(NO3)3+4^H2O. 

Very  deliquescent.  Easily  sol.  in  H2O  and 
absolute  alcohol.  (Winkler.) 


Iron  (ferrous)  nitrate,  Fe(NO8)2+6H2O. 

100  pts.  of  crystals  dissolve  in  50  pts.  H2O 
at  0°,  sp.  gr.  of  solution  =  1.44;  40.8  pts.  H2O 
at  15°,  sp.  gr.  of  solution  =  1.48;  33.3  pts.  H2O 
at  25°,  sp.  gr.  of  solution  =  1.50.  (Ordway, 
Sill.  Am.  J.  (2)  40.  325.) 

Sat.  solution  contains  at: 
—9°      0°      +18°    24°   60.5°  Mpt. 
39.68   41.53  45.14  46.51   62.50%  Fe(NO3)2. 
(Funk,  Z.  anorg.  1899,  20.  406.) 

Sat.  solution  of  Fe(NO3)2+6H2O  in  H2O 
contains  41.5%  Fe(NO3)2  at  0°;  45.1%  at  18°. 
(Mylius,  Z.  anorg.  1912,  74.  411.) 


568 


NITRATE,  IRON,  BASIC 


+9H2O.    Solubility  in  H2O. 

Sat.  solution  contains  at: 
—27°    —21.5°    —19°    —15.5° 
35.66         36.10    36.56        37.17%  Fe(NO3)2. 

Cryohydrate  is  formed  at  — 28°.  (Funk, 
Z.  anorg.  1899,  20.  407.) 

Fe(NO3)2-|-Aq  decomposes  on  heating;  less 
rapidly  when  dil.,  more  readily  in  presence  of 
excess  of  acid.  (Ordway.) 

Iron  (ferric)  nitrate,  basic,  36Fe2O3,  N2O5+ 

48H2O  (?). 

Easily  sol.  in  H2O.  SI.  sol.  in  dil.  HN03-f 
Aq;  very  si.  sol.  in  alcohol.  (Hausmann,  A. 
89.  111.) 

8Fe2O3,  N2O5+12H2O.  SI.  sol.  in  H2O; 
very  si.  sol.  in  cold  or  warm  dil.  HNO3  + 
Aq;  more  easily  sol.  in  hot  HCl+Aq.  (Haus- 
mann.) 

-f-#H2O.  Sol.  in  H2O;  completely  pptd. 
from  aqueous  solution  by  NaCl,  NH4C1,  KI, 
KC1O3,  Na2SO4,  CaSO4,  ZnSO4,  CuSO4,  KNO3 
NaNO3,  Ba(C2H3O2)2,  or  Zn(C2H3O2)2+Aq. 
More  slowly  pptd.  by  NH4NO3,  Mg(NO3)2, 
Ba(NO8)2,  or  Pb(NO3)2+Aq.  Not  pptd.  by 
alcohol,  Pb(C2H3O2)2,  Cu(C2H3O2)2,  Hg(CN)2, 
AgNO3,  or  As2O3+Aq.  (Ordway,  Sill.  Am. 
J.  (2)  9.  30.) 

4Fe2O3,  N2O5+1^H2O.  Easily  sol.  in 
H2O;  si.  sol.  in  dil.  HNO3-f  Aq,  and  in  al- 
cohol. (Hausmann.) 

+3H20.  Insol.  in  H2O  or  HNO3+Aq;  sol. 
in  HCl+Aq.  (Scheurer-Kestner,  C.  R.  87. 
927.) 

+9H2O.  Not  deliquescent;  easily  sol.  in 
H2O.  (Ordway.) 

3Fe2O3,  N2O5+2H2O.  Insol.  in  H2O. 
(Scheurer-Kestner.) 

2Fe2O3,  N2O6+H2O.     Decomp.  by  H2O. 
(Scheurer-Kestner. ) 
+8H2O.    (S.-K.) 

Fe2O3,  N2O6.    Decomp.  by  H2O.    (S.-K.) 
Fe2O3,  2N2O5.    Sol.  in  H2O  or  alcohol  in 
all  proportions.    Insol.  in  HNO3+Aq. 

N2O6  with  1,  2,  3,  4,  5,  6,  and  8Fe2O3 
forms  compounds,  sol.  in  H2O.  (Ordway.) 

Solubility  determinations  show  that  there 
are  no  definite  basic  nitrates  of  iron  formed 
from  solutions  at  25°,  and  that  the  solid  phase 
under  these  conditions  is  a  solid  solution  of 
Fe2O3,  HNO3  and  H2O.  The  normal  salt, 
Fe2O3,  3N2O5,  18H2O  is  stable  in  solutions 
containing  about  30-45%  N2O8.  In  higher 
concentrations  of  nitric  acid  it  appears  to  be 
metastable  and  a  new  salt,  Fe2O3,  4N2O5, 
18(?)H2O  is  the  stable  form.  (Cameron,  J. 
phys.  Chem.  1909,  13.  252.) 

Iron  (ferric)  nitrate,  Fe(NO3)3. 

+H2O.  (Scheurer-Kestner,  A.  ch.  (3)  65. 
113.) 

+6H2O.  Deliquescent,  and  sol.  in  any 
amount  of  H2O.  (Schonbein,  Pogg.  39.  141.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 


+9H2O.  Deliquescent.  Sol.  in  H2O  and 
alcohol.  SI.  sol.  in  HNO3+Aq.  2  pts.  salt 
with  1  pt.  H2O  lower  the  temperature  18.5°. 
(Scheurer-Kestner.) 

Sp.  gr.  of  solution  at  17.5°  containing: 
5        10        15        20        25%  Fe(NO3)3, 
1.0398  1.0770  1.1182  1.1612  1.2110 

30  35  40  45  50%  Fe(NO3)3, 
1.2622  1.3164  1.3746  1.4338  1.4972 

55  60  65%  Fe(NO3)3. 

1.5722     1.6572     1.7532 

(Franz,  J.  pr.  (2)  5.  274.) 

Nearly  insol.  in  cone.  HNO3+Aq  at  temp, 
below  15.5°. 

Easily  sol.  in  alcohol. 

Melts  in  crystal  H2O  at  47.2°.    (Ordway.) 

Sat.  Fe(NO3)3-hAq  boils  at  125°.  (Ord- 
way.) 

Lanthanum  nitrate,  La(NO3)3+6H20. 

Very  deliquescent;  easily  sol.  in  H2O  and 
alcohol.  (Mosander.)  Melts  in  its  crystal 
H2O  at  40°;  boils  at  124.5°.  (Ordway.) 

La(NO3)3+Aq  sat.  at  25%  contains  60.17% 
La(NO3)3,  or  100  g.  H2O  dissolve  151.1  g. 
La(NO3)3  at  25°.  (James  and  Whittemore, 
J.  Am.  Chem.  Soc.  1912,  34.  1169.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328;  Eidmann,  C.  C.  1899,  II.  1014.) 

Lanthanum  magnesium  nitrate,  2La(N03)3, 
3Mg(NO3)2+24H2O. 

Deliquescent  in  moist  air.  (Holzmann,  J. 
pr.  75.  350.) 

1  1.  sat.  solution  in  HN03+Aq  (sp.  gr. 
1.325)  contains  63.8  g.  hydrous  salt  at  16°. 
(Jantsch,  Z.  anorg.  1912,  76.  321.) 

Lanthanum  manganous  nitrate,  2La(NO3)3, 

3Mn(NO3)2+24H2O. 
Sol.  in  H2O.    (Damour  and  Deville.) 
1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 

1.325)  contains  193.1  g.  hydrous  salt  at  16°. 

(Jantsch.) 

Lanthanum  nickel  nitrate,  2La(NO3)3, 
3Ni(NO3)2+36H2O. 

Very  sol.  in  H2O.  (Frerichs  and  Smith,  A. 
191.  355.) 

+24H2O.  1  1.  sat.  S9lution  in  HN03+ 
Aq  (sp.  gr.  1.325)  contains  80.3  g.  hydrous 
salt  at  16°.  (Jantsch.) 

Lanthanum  rubidium  hydrogen  nitrate, 

[La(NO3)4]Rb,  HNO3+6H2O. 
Sol.  in  H2O  and  HNO3.    (Jantsch,  Z.  anorg. 
1911,  69.  225.) 

Lanthanum  thallous  nitrate,  [La(NO3)5]Tl24- 

4H20. 

Hydroscopic.  (Jantsch,  Z.  anorg.  1911,  69. 
228.) 


NITRATE,  LEAD 


569 


Lanthanum       zinc       nitrate,       2La(NO3)3, 

Solubility  in  100  pts.  H2O  at  t°. 

3Zn(NO3)2+24H2O. 

* 

Very  sol.  in  H2O.    (Damour  and  Deville,  J. 
B.  1858.  135.) 

t° 

Pts. 
Pb(N03)2 

t° 

Pts. 
Pb(NO»)2 

t° 

Pts. 
Pb(NO3)2 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  124.1  g.  hydrous  salt  at  16°. 
(Jantsch,  Z.  anorg.  1912,  76.  321.) 
+69H2O.     (Frerichs  and  Smith,  A.   191. 

or*-   \ 

0 
1 
2 
3 

36.5 
37.4 
38.3 
39.1 

36 
37 
38 
39 

65.9 
66.7 
67.6 
68.5 

72 
73 
74 
75 

99.7 
100.7 
101.7 
102.6 

o5o.) 

4 

39.8 

40 

69.4 

76 

103.6 

5 

40.5 

41 

70.3 

77 

104.6 

Lead   nitrate,    basic,    2PbO,    N2O5+H2O  = 
Pb(OH)NO3. 

6 

7 
8 

41.2 
42.0 

42.8 

42 
43 
44 

71.2 
72.1 
73.0 

78 
79 
80 

105.6 
106.6 
107.6 

Sol.  in  5.15  pts.  H2O  at  19.2°.    (Pohl,  W.  A. 
B.  6.  597.)    Very  si.  sol.  in  cold,  much  more 
inhotH2O.    (Berzelius.)    Sol.  inPb(C2H3O2)2 

9 
10 
11 

43.6 
44.4 
45.2 

45 

46 
47 

74.0 
74.9 
75.9 

81 

82 
83 

108.6 
109.6 
110.6 

+Aq.   .(Guignet,  C.  R.  56.  358.) 
Insol.  in  H2O;  sol.  in  acids.     (Athanesco, 

12 
13 

46.0 
46.8 

48 
49 

76.8 

77.7 

84 
85 

111.5 
112.5 

Bull.  Soc.  1895,  (3)  13.  178.) 

14 

47.5 

50 

78  7 

86 

113.5 

+2H2O.    (Andre,  C.  R.  100.  639.) 

15 

48.3 

51 

79.6 

87 

114.5 

3PbO,  N2O6+13^H2O.  SI.  sol.  in  pure  H2O. 

16 

49.1 

52 

80.5 

88 

115.4 

Insol.  in  H2O  containing  HC1.    (Berzelius.) 

17 

49.9 

53 

81.5 

89 

116.4 

+3H2O.    Sol.  in  119.2  pts.  cold,  and  10.5 

18 

50.7 

54 

82.4 

90 

117.4 

pts.  boiling  H2O.    Sol.  in  Pb(C2H3O2)2+Aq, 

19 

51.5 

55 

83.3 

91 

118  4 

but  si.  sol.  in  KNO3+Aq.    (Vogel,  jr.  A.  94. 

20 

52.3 

56 

84.3 

92 

119.4 

97.) 

21 

53.1 

57 

85.2 

93 

120.3 

=  lOPbO,  3N2O5  -f  5H2O.    (Wakemann  and 

22 

53.9 

58 

86.1 

94 

121.3 

Wells,  Am.  Ch.  J.  9.  299.) 

23 

54.7 

59 

87.1 

95 

122  3 

+4H2O.    (Andre,  C.  R.  100.  639.) 
6PbO,  N2O5-hH2O.    Nearly  insol.  in  H2O. 

24 
25 

55.6 
56.4 

60 
61 

88.0 
89.0 

96 
97 

123.2 
124.2 

(Lowe,  J.  pr.  98.  385.) 
lOPbO,  3N2O5+4H2O.     Less  sol.  in  H2O 

26 

27 

57.3 
58.1 

62 
63 

90.0 
90.9 

98 
99 

125.2 
126  1 

than  Pb(NO3)OH,  and  not  decomp.  by  boiling 

28 

59.0 

64 

91.9 

100 

127.0 

H2O.    (Wakemann  and  Wells,  Am.  Ch.  J.  9. 

29 

59.8 

65 

92.8 

101 

128.0 

299.) 

30 

60.7 

66 

93.8 

102 

128.9 

31 

61.6 

67 

94.8 

103 

129.9 

32 

62.4 

68 

95.7 

104 

130  9 

Lead  nitrate,  Pb(NO3)2. 

33 

63.3 

69 

96.7 

104.7 

131.5 

Sol.  in  H2O  with  absorption  of  much  heat. 

34 

64.1 

70 

97.7 

(Rose.) 

35 

65.0 

71 

98.7 

1  pt.  Pb(NO3)2  dissolves  in  7Y2  pts.  cold  H2O. 
(Mitscherlich.) 

1  pt.  Pb(NO3)2  dissolves  in  1.989  pts.  H2O  at  17.5° 
and  forms  a  liquid  of  1.3978  sp.  gr.  (Karsten.) 

1  pt.  Pb(NO3)2  dissolves  in  1.707  pts.  H2O  at  22.3°; 
in  1.585  pts.  H2O  at  24.7°.  (Kopp.) 

Sol.  in  1.87  pts.  H2O  at  17.5°.     (Schiff,  A.  109.  326.) 

100  pts.  Pb(NO$)2+Aq  sat.  at  102.2°  contain  52.5 
pts.  Pb(NO3)2,  or  100  pt.  H2O  dissolve  110.526  pts. 
Pb(NO3)2at  102.2°.  (Griffiths.) 

Sol.  in  7.5  pts.  cold  H2O  and  much  less  hot  H2O. 
(Wittstein.) 

100  Dts.  boiling  H2O  dissolve  13  pts.  Pb(NOs)2. 
(Ure's  Diet.) 

100  pts.  Pb(NO3)2+Aq  sat.  at  19-20°  con- 
tain 35.80  pts.  salt.  (v.  Hauer,  W.  A.  B.  53,  2. 
221.) 

1  pt.  dissolves: 

at  0°  10°  25°  45°  65°  85°  100° 
in  2.58  2.07  1.65  1.25  0.99  0.83  0.72  pts.  H2O. 

(Kremers,  Pogg.  92.  497.) 


1  1.  Pb(NO3)2+Aq  sat.  at  15°  contains 
461.49  g.  Pb(NO3)2  and  928.58  g.  H2O,  and 
has  sp.  gr.  1.39.  (Michel  and  Krafft,  A.  ch. 
(3)  41.  471.) 


(Mulder,  Scheik.  Verhandel.  1864.  66.) 


100  g.  H2O  dissolve  52.76  g.  Pb(NO3)2  at 
17°.  (Euler,  Z.  phys.  Ch.  1904,  49.  315.) 

Solubility  of  Pb(NO3)2  in  H2O  at  20°  = 
1.52  g.  mol.  per  1.  Sp.  gr.  of  sat.  solution  = 
1.419.  (Fedotieff,  Z.  anorg.  1911,  73.  178.) 

Sat.  Pb(NO3)2+Aq  at  0°  contains  26.7% 
Pb(NO3)2;  at  18°,  29.1%  Pb(NO3)2.  (Mylius, 
Z.  anorg.  1912,  74.  411.) 


Sp.  gr.  of  Pb(NO3)2+Aq  at  19.5°. 


% 

PbCNOsh 

Sp.gr. 

Pb(NOi)i 

Sp.  gr. 

5 
10 
15 
20 

1.045 
1.093 
1.144 
1.203 

25 
30 
35 

1.266 
1.334 
1.414 

(Kremers,  calculated  by  Gerlach,  Z   anal   8 

286.) 


570 


NITRATE,  LEAD 


Sp.  gr.  of  Pb(NO3)2+Aq  at  17.5°. 


Pb(NO3)2 

Sp.  gr. 

% 
Pb(N03)2 

Sp.  gr. 

5 
10 
15 
20 

1.044 
1.092 
1.144 
1.200 

25 
30 
35 

sat.  sol. 

1.263 
1.333 
1.409 
1.433 

(Gerlach,  Z.  anal.  27.  283.) 

Sp.  gr.  of  Pb(NO3)2+Aq  sat.  at  8C 
(Anthon.) 


1.372, 


Sp.  gr.  of  Pb(NO3)2+Aq  at  17.5°. 


Pb(NO3)2 

Sp.  gr. 

Pb(NOs)2 

Sp.  gr. 

1 

1.0080 

20 

1.1902 

2 

1.0163 

21 

.2016 

3 

1.0247 

22 

.2132 

4 

1.0331 

23 

.2251 

5 

1.0416 

24 

.2372 

6 

1.0502 

25 

.2495 

7 

1.0591 

26 

.2620 

8 

1.0682 

27 

1.2747 

9 

1.0775 

28 

1.2876 

10 

1.0869 

29- 

1.3907 

11 

1.0963 

30 

1.3140 

12 

1  .  1059 

31 

1.3276 

13 

1.1157 

32 

1.3416 

14 

1  .  1257 

33 

1.3558 

15 

1  .  1359 

34 

1.3702 

16 

1  .  1463 

35 

1.3848 

17 

1  .  1569 

36 

1.3996 

18 

1.1677 

37 

1.4146 

19 

1.1788 

(Schiff,   calculated  by  Gerlach,   Z.   anal.  8. 
286.) 

Sp.  gr.  of  Pb(NO3)2+Aq  at  t°. 


t° 

%  Pb(N03)2 

Sp.  gr. 

14 

5 

1.0451 

14 

10 

1.0939 

14.5 

15 

1  .  1468 

14.3 

20 

1.2045 

15 

25 

1.2678 

15 

32.28 

1.3716 

(Long,  W.  Ann.  1880,  11.  40.) 

Sp.  gr.  of  Pb(NO3)2+Aq  at  room  temp, 
containing: 

17.93         32.22%  Pb(NO8)2. 
1.1786         1.3619 
(Wagner,  W.  Ann.  1883,  18.  267.) 
Sp.  gr.  of  Pb(NO3)2+Aq  at  25°. 


Concentration  of 

Pb(NO3)2+Aq 

Sp.  gr. 

1-normal 
Vr-       " 
Vc-      " 

Vs-       " 

1.1380 
1.0699 
1.0351 
1.0175 

(Wagner,  Z.  phys.  Ch.  1890,  6.  36.) 

Pb(NO3)2+Aq  containing  15.93%  Pb(NO3)2 

has  sp.  gr.  20/°20°  =  1.1558. 
Pb(NO3)2+Aq  containing  30.57%  Pb(NO3)2 

has  sp.  gr.  20°/20°  =  1.3436. 
Pb(NO3)2+Aq  containing  30.69%  Pb(NO3)2 
has  sp.  gr.  20°/20°  =  1.3465. 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  279.) 

Sat.  Pb(NO3)2+Aq  boils  at  103.5°.  (Krem- 
ers.) 

Sat.  Pb(NO3)2+Aq  boils  at  102.2°,  and 
contains  140  pts.  Pb(NO3)2  to  100  pts.  H2O. 
(Griffiths.) 

Sat.  Pb(NO3)2+Aq  boils  at  103.5°.  (Ger- 
lach,  Z.  anal.  26.  427.) 

B.-pt.  of  Pb(NO3)2+Aq  containing  pts. 
Pb(NO3)2  to  100  pts.  H2O,  according  to 
Gerlach  (Z.  anal.  26.  449). 


B.-pt. 

Pts. 
Pb(NO3)2 

B.-pt. 

Pts. 
Pb(NOs)2 

100.5° 
101 
101.5 
102 

11 

26 
44 
65 

102.5° 
103 
103.5 

87 

111 

137 

Insol.  in  cone.  HNO3+Aq. 

Solubility  of  Pb(NO3)2+Ba(NO3)2, 

See  under  Ba(NO3)2. 

Solubility  of  Pb(NO3)2+Cu(NO3)2. 

See  under  Cu(NO3)2. 

Sol.  in  sat.  KNO3+Aq  without  pptn.,  100 
pts.  H20  at  18.75°  dissolving  114  pts.  mixed 
salt,  viz.  84.1  pts.  Pb(NO3)2  and  29.9  pts. 
KNO3.  (Karsten.) 

100  pts.  H2O  dissolve  119.6  pts.  Pb(NO3)2 
and  67.1  pts.  KNO3  at  21.2°.  (Riidorff,  B.  6. 
484.) 

100  g.  H2O  dissolve  95.39  g.  Pb(NO3)2  and 
61.05  g.  KNO3  at  20°.  (Le  Blanc  and  Noyes. 
Z.  phys.  Ch.  1890,  6.  386.) 

Sol.  in  sat.  NaNO3+Aq  without  pptn.,  100 
pts.  H2O  at  18.75°  dissolving  121.9  pts.  mixed 
salt,  viz.  87.8  pts.  Pb(NO3)2  and  34.1  pts. 
NaNO3.  (Karsten.) 

Solubility  of  Pb(N08)2+NaNO8. 


Solid  phase  =  Pb(NO3)2. 


t°  of  saturation 

%  NaNOs 

%  Pb(N03)2 

32 

34.42 

19.69 

35.5 

34.15 

20.33 

39.5 

33.71 

21.35 

44. 

33.35 

22.19 

49.1 

32.94 

23.15 

55 

32.60 

23.93 

58 

32.47 

24.24 

62 

32.33 

24.57 

65 

32.14 

24.89 

NITRATE,  NITRITE,  LEAD,  BASIC 


571 


Solubility  of  Pb(NO3)2+XaNO3—  Continued. 

Solubility  of  Pb(NO3)2  in  pyridine  at  t°. 

Solid  phas 

e  =  NaNO3 

t° 

G.Pb(NOs)2 
per  100  g. 
CoH6N 

Solid  phase 

t°  of  saturation 

%  NaNOs 

%  Pb(NO3)2 

21 
26.5 
31 

38.8 
41 
44.25 
51 
58 
64 

40 
•      42 
43 
44 
45 
46 
47 
49 
49 

.97 
.04 
.18 
.63 
.11 
.03 
.28 
.03 
.92 

13.62 
13.38 
12.88 
12.78 
12.94 
12.45 
12.50 
11.76 
11.56 

—19.4 
—14.5 
—10 
0 
5.4 
8.7 
14.72 
19.97 
24.75 
30.03 
34.97 
40.03 
45. 
49.97 
51  tr.  pt. 
59.52 
70 
80 
89.93 
94.94 
96  tr.  pt 
99.89 
104.90 
109.90 

2.93 
2.14 
1.90 
3.54 
3.93 
5.39 
6.13 
6.78 
8.56 
10.98 
13.20 
16.94 
22.03 
29.37 

36]  70 
47.29 
61.60 
90.21 
128.06 

143]  36 
152 
163.80 

Pb(NO3)2,(4C5H6N 

u 

t( 
tt 

t( 
it 
(t 

1C 
11 
(( 
It 
(I 
{( 

"+Pb(N03)2,  3C5H6N 

Pb(NO3)2,  3C6H5N 
ft 

d 

1C 

{( 

"+Pb(N03)2,  2C6H5N 

Pb(NO3)2,  2C5H5N 
it 

u 

(Isaac,  Chem.  Soc.  1908,  93.  398.) 

Also  sol.  in  KNO3+NaNO3+Aq. 
100    pts.    sat.    Pb(NO3)2+Sr(N03)2+Aq 
contain  45.98  pts.  of  the  two  salts  at  19.20°. 
(v.  Hauer,  J.  pr.  98.  137.) 

Solubility  of  Pb(N03)2+Sr(NO3)2  at  25°. 

G.  per 

100  cc. 

Mol.  per  cent 

in  solid  phase 

Pb(NO3)2 

Sr(N03)2 

Pb(NOs)2 

Sr(NO3)2 

46.31 
50.47 
53.92 
45.34 
44.48 
25.23 
19.13 
0 

0 
4.56 
8.14 
17.81 
18.74 
35.03 
37.54 
71.04 

100. 
99.05 
98.11 
97.02 
96.06 
83.84 
32.88 
0 

0 
0.95 
1.89 
2.98 
3.94 
16.16 
67.12 
100. 

(Walton  and  Judd,  J.  Am.  Chem.  Soc.  1911, 
33.  1036.) 

Lead  mercurous  nitrate,  2PbO,  2Hg2O,  3N2O5. 
Decomp.  by  H2O.    Sol.  in  warm  dil.  HNO3, 
or  Hg2(NO3)2+Aq  without  decomp.     (Stad- 
eler,  A.  87.  129.) 

Lead  silver  nitrate,  Pb(NO3)2,  2AgNO3. 
Sol.  in  H2O.    (Sturenberg,  Pogg.  74.  115.) 

(Fock, 

Z.  Kryst. 

Min.  1897,  28.  365.) 

Very  easily  sol.  in  liquid  NH3.  (Franklin 
Am.  Ch.  J.  1898,  20.  828.) 

100  pts.  alcohol  of  0.9282  sp.  gr.  dissolve: 
at  4°  8°  22°  40°  50° 

4.96  5.82  8.77  12.8  14.9  pts.  Pb(NO3)2 
(Gerardin,  A.  ch.  (4),  5.  129.) 


100  pts.  absolute  methyl  alcohol  dissolv< 
1.37  pts.  at  20.5°. 

100  pts.  absolute  ethyl  alcohol  dissolve  0.04 
pt.  at  20.5°.  (de  Bruyn.  Z.  phys.  Ch.  10 
783.) 

Very  si.  sol.  in  acetone.  (Krug  and  M'El- 
roy,  J.  Anal.  Ch.  6.  184.) 

Insol.  in  cold,  si.  sol.  in  hot  CS2.  (Arctow- 
ski,  Z.  anorg.  1894,  6.  257.) 

Insol.  in  benzonitrile.  (Naumann,  B.  1914 
47.  1370.) 

Insol.  in  methyl  acetate.  (Naumann,  B 
1909,  42.  3790);  ethyl  acetate.  (Naumann 
B.  1910,  43.  314.) 

Mol.  weight  determined  in  pyridine.  (Wer- 
ner, Z.  anorg.  1897,  16.  21.) 


Lead  silver  nitrate  iodide,  Pb(NO3)2, 8AgNO3, 

4AgI. 

Decomp.  by  H2O.    (Sturenberg.) 
Pb(NO3)2,  2AgNO3,  2AgI.     Decomp.  by 

H2O.    (Sturenberg.) 

Lead  nitrate  nitrite,  basic,  4PbO,  N2O5,  N2O3 

+2H2O=Pb(OH)NO8,  Pb(OH)NO2. 
SI.  sol.  in  cold,  easily  in  hot  H2O.    Sol.  in 
80  pts.  H2O  at  23°  (Chevreuil);  85  pts.  at  ord. 
temp.  (Bromeis,  A.  72.  38);  10.6  pts.  at  100° 
(Chevreuil). 


+2H20. 


Solubility  in  acetic  acid. 


Normality 
of  acid 

g.  PbO  per 
100  cc.  sat. 
solution 

Normality 
of  acid 

g.  PbO  per 
100  cc.  sat. 
solution 

0 
0.05 
0.10 

0.601 
1.323 
2.185 

0.25 
0.50 
0.75 

5.450 
9.690 
15.874 

(Chilesotti,  Att.  Acad.  Line.  1908,  (5)  17,  II. 

475.) 


572 


NITRATE,  LEAD,  PHOSPHATE 


Formula  is  3Pb(OH)NO3,  5Pb(OH)NO2  + 
H2O.  (v.  Lorenz,  W.  A.  B.  84,  2.  1133.) 

+3H2O.    (v.  Lorenz.) 

4PbO,  N2O5,  3N2O3+4H2O.  Sol.  in  H20 
(Bromeis.) 

6PbO,  N2O6, 2N2O3+32/3H2O=Pb(OH)NO3 
2Pb(OH)NO2+2/3H2O.  (v.  Lorenz.) 

6PbO,  2N2O6,  N2O3  +  32/3H2O  = 
2Pb(OH)NO3,  Pb(OH)NO2+V3H2O.  (v 
Lorenz.) 

7PbO,  N2O3,  N2O5+3H2O.  Less  sol.  in 
H2O  than  4PbO,  N2O5,  N2O3+2H2O;  sol.  in 
cold  cone.  HNO3+Aq.  (Peligot,  A.  39.  338.) 

8PbO,  N2O5, 3N2O3+42/3H2O=Pb(OH)NO3 
3Pb(OH)NO2  +  V3H2O.  (v.  Lorenz.) 

lOPbO,  N205, 4N203+5H20  =  Pb(OH)N03 
4Pb(OH)NO2.  (v.  Lorenz.) 

12PbO,N2O6,5N2O3+6H2O  =  Pb(OH)NO3, 
5Pb(OH)NO2.  (v.  Lorenz.) 

10PbO,5N2O6,2N2O3+4H20=Pb(OH)N03, 
2Pb(OH)NO2,  2PbO  +  3^H2O.  (v.  Lorenz.) 

14PbO,  N2O6, 3N2O3+6H2O=Pb(OH)NO3, 
3Pb(OH)NO2,  3PbO+H2O.  (Bromeis.) 

14PbO,  3N2O5,  N2O3+6H2O  = 
3Pb(OH)NO3,     Pb(OH)NO2,     3PbO+H2O. 
(Bromeis.) 

16PbO,  2N2O5,  3N2O3+6H2O  = 
4Pb(OH)N03,  6Pb(OH)N02,  5PbO,  Pb(OH)2 
(v.  Lorenz.) 

16PbO,  3N2O5,  5N2O3+10H2O  = 
3TPb(OH)NO3,      5Pb(OH)NO2+H2O.        (v. 
Lorenz.) 

26PbO,  6N2O5,  7N203-}-21H2O  = 
6Pb(OH)NO3,     7Pb(OH)NO2+4H2O.       (v. 
Lorenz.) 

Lead  nitrate  phosphate,  Pb(NO3)2,  Pb3(PO4)2 

+2H20. 

Completely  insol.  in  cold  H2O.  Decomp.  by 
boiling  H2O  into  its  constituents.  Sol.  in  a 
little  cone.  HNO3+Aq  without  decomp. 
(Gerhardt,  A.  72.  83.) 

Lead  nitrate  phosphite,  Pb(NO3)2,  PbHPO3. 
Decomp.  by  H2O.  Sol.  in  Pb(NO3)2+Aq. 
Pb(NO3)2+Aq  (33.3  g.  per  litre)  dissolves  1 
g.  salt  at  15°.  If  less  than  31  g.  per  litre  of 
Pb(NO3)2  are  present  the  salt  is  decomp. 
(Amat,  A.  ch.  (6)  24.  317.) 

Lead  nitrate  potassium  nitrite.  Pb(NO3)2, 
2KN02+H20. 

Difficultly  sol.  in  H2O.  (Lang,  J.  B.  1862. 
102.) 

3PbO,  3K20,  4N203,  2N2O5+3H2O.  Sol. 
in  H2O.  (Hayes,  Sill.  Am.  J.  (2)  31.  226.) 

Lithium  nitrate,  LiNO3. 

Very  deliquescent,  and  sol.  in  H2O. 
100  pts.  H2O  dissolve: 
at  0°  20°  40°      70°    100°   110° 
48.3  75.7  169.4  196.1  227.3  256.4  pts.  LiNO3. 
(Kremers,  Pogg.  99.  47.) 


Forms  supersaturated  solutions  with  ease, 
which  crystallize  when  temp,  is  lowered  to 
+  1°.  (Kremers,  Pogg.  92.  520.) 

Sat.  solution  boils  at  over  200°.  (Kremers, 
Pogg.  99.  43.) 

1  pt.  LiNO3  dissolves  in  200  pts.  HNO3. 
(Schultz,  Zeit.  Ch.  (2)  5.  531.-) 

100  pts.  of  the  sat.  solution  contain  at: 

64.2°        70.9° 

64.9          66.1  pts.  anhydrous  salt. 
(Donnan  and  Burt,  Chem.  Soc.  1903,  83. 
339.) 
See  +^H2O,  and  3H20. 


Sp.  gr.  of  LiNO3-f-Aq  at  19.5°  containing 
pts.  LiN03  in  100  pts.  H2O: 


12.7 
1.069 

54.8 
1.245 


14.2 
1.077 

57.5 
1.255 


26.4 
1.134 

77.4 
1.315 


41.8  pts.  LiNO3, 
1.197 

79.4  pts.  LiNO3. 
1.319 


(Kremers,  Pogg.  114.  45.) 


Sp.  gr.  of  LiN03+Aq. 


g.  LiNOs  in  1000  g. 
of  solution 

Sp.  gr.  16/16° 

0 
4.8526 
10.9128 
17.9016 

1.000000 
1.002469 
1  .  0055495 
1.009113 

(Dijken,  Z.  phys.  Ch.  1897,  24.  109.) 


Sp.  gr.  20°/4°  of  a  normal  solution  of  LiNO3 
=  1.03803;  of  a  0.5-normal  solution  =  1.01830. 
(Haigh,  J.  Am.  Chem.  Soc.  1912,  34.  1151.) 

Very  easily  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  828.) 

Sol.  in  strong  alcohol. 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4328.) 

Solubility  in  acetone  =  0.343  g.  mol.  per  1. 
at  18°.  (Roshdestwensky  and  McBride, 
Chem.  Soc.  1911,  99.  2140.) 

Insol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1370.) 

Difficultly  sol.  in  ethyl  acetate.  (Nau- 
mann, B.  1910,  43.  314.) 

+  ^H2O.    Solubility  in  H2O. 

100  pts.  of  the  sat.  solution  contain  at : 

43.6°    50.5°    55.0°    60.0° 

60.8     61.3     63.0     63.6  pts.  anhydrous  salt. 


61.1°  is  the  temp,  at  which  LiNO3 
goes  over  into  LiNO3.     (Donnan  and  Burt, 
'"'hem.  Soc.  1903,  83.  339.) 


NITRATE,  MAGNESIUM 


573 


+3H20. 
Solubility  in  H2O. 

100  pts.  of  the  sat.  solution  contain  pts. 
anhydrous  salt  at  t°. 

Sp.  gr.  of  Mg(NO3)2+Aq  at  21°. 

%  Mg(N03)2 

+oH2O 

Sp.  gr. 

%Mg(N03)2 

Sp.  gr. 

2 

4 
6 
8 
10 
12 
14 
16 
18 
20 
22 
24 
26 

.0078 
.0158 
.0239 
.0321 
.0405 
.0490 
.0577 
.0663 
.0752 
.0843 
1.0934 
1  .  1026 
1.1120 

28 
30 
32 
34 
36 
38 
40 
42 
44 
46 
48 
50 

1.1216 
1.1312 
1.1410 
1.1508 
1.1608 
1.1709 
1.1811 
1.1914 
1.2019 
1.2124 
1.2231 
1.2340 

t° 

Pts.  anhydrous  salt 

0.10 
10.50 
12.10 
13.75 
19.05 
22.10 
27.55 
29.47 
29.78 
29.87 
29.86 
29.64 
29.55 

34.8 

37.9 
38.2 
39.3 
40.4 
42.9 
47.3 
53.67 
55.09 
56.42 
56.68 
57.48 
58.03 

(Schiff,   calculated  by  Gerlach,  Z.  anal.  8. 

286.) 

Sp.  gr.  of  Mg(NO3)2+Aq  at  18°. 

Mpt.  of  LiNO3+3H2O  is  29.88°. 

(Donnan  and  Burt,  Chem.  Soc.  1903, 
83.  337.) 

IMTarrmAciiiifft    vti+^/t+n      Vi«nl««        \  I  .  .-    AT    I    \ 

%  Mg(NOa)s 

Sp.  gr. 

%  Mg(N03)2 

Sp.  gr. 

5 
10 

1.0378 
1.0763 

15 

17 

1.1181 
1.1372 

A»A  W^AAWOA  W.J..1.A     .LUtA  ClL\s}      ILT«.OXV/y      iTj.  ^3 X  1   ^^  O* 

Insol.  in  H2O  and  alcohol.  Sol.  in  acids. 
(Chodnew,  A.  71.  241.) 

+5H2O.  Decomp.  by  H2O.  (Didier,  C.  R. 
1896,  122.  936.) 

Magnesium  nitrate,  Mg(N03)2. 
Anhydrous.    Deliquescent. 

Sol  in  1  pt.  H2O  at  15.6°.  Sol.  in  4  pts.  abs.  alcohol 
at  15.6°,  and  2  pts.  at  boiling  temp.  More  sol.  in  alcohol 
of  0.817  sp.  gr.  than,in  that  of  0.900.  (Kirwan.) 

Sol.  in  0.3458  pt.  strong  alcohol  at  82.5°.     (Wenzel.) 
Sol.  in  10  pts.  strong  alcohol  at  15°.     (Bergmann.) 
Sol.  in  9  pts.  stiong  alcohol  on  heating.     (Bergmann.) 

Solubility  in  H2O  in  .presence  of  the  an- 
hydrous salt. 

Sat.  solution  contains  at: 


89° 
63.14 


77.5° 
65.67. 


67' 


67.55%  Mg(N03)2. 
(Funk,  Z.  anorg.  1899,  20.  396.) 
See  +6,  and  9H2O. 

Sp.  gr.  of  Mg(NO3)2+Aq  at  14°. 


%  Mg(NOs)«» 
6H20 

Sp.  gr. 

%  Mg(N03)2, 
6H20 

Sp.  gr. 

1 

5 
10 
15 
20 
25 

1.0034 
1.0202 
1.0418 
1.0639 
1.0869 
1.1103 

30 
35 
40 
45 

49 

1.1347 
1.1649 
1  .  1909 
1.2176 
1.2397 

(Oudemans,  Z.  anal.  7.  419.) 


(Kohlrausch,  W.  Ann.  1879.  1.) 

Sp.  gr.  of  Mg(NO3)2-f  Aq  at  room  temp, 
containing: 

18.62       34.19       39.77%  Mg(N03)o. 
1.1025      1.2000      1.4298 
(Wagner,  W.  Ann.  1883,  18.  273.) 

Sp.  gr.  of  Mg(NO8)2+Aq  at  25°. 


Concentration  of 
Mg(N03)2+Aq 

Sp.  gr. 

1-normal 

Vr-      " 
l/«-      " 

Ys-     " 

1 
1 
1 
1 

.0512 
.0259 
.0130 
.0066 

(Wagner,  Z.  phys.  Ch.  1890,  5.  38.) 

Sp.  gr.  of  solution  sat.  at  18°  =  1.384,  con- 
taining 43.1%  Mg(NO3)2.  (Mylius,  B.  1897, 
30.  1718.) 

Sp.  gr.  of  Mg(NO3)2+Aq. 


M  Mg(NOs)2  g.  in  1000  g. 
of  solution 

Sp.  gr.  16°/16° 

0 

1.000000 

0.8099 

1.000660 

1.5621 

.001253 

3.3398 

.  002539 

7.4410 

.  005523 

15.161 

.011151 

29.356 

.021580 

58.353 

.043329 

81.025 

.060773 

(Dijken,  Z.  phys.  ( 

Uh.  1897,  24.  107.) 

574 


NITRATE,  MAGNESIUM  NEODYMIUM 


Sp.  gr.  of  Mg(NO3)2+Aq  at  20. 1°. 
p  =  per  cent  strength  of  solution;  d  =  ob- 
served density;  w  =  volume  concentration  in 


grams  per  cc. 


p 

d 

w 

35.02 

1.3110 

0.46695 

31.15 

1.2655 

0.39420 

25.03 

1.2057 

0.30172 

19.55 

.1551 

0.22585 

13.43 

.  1028 

0.14815 

10.09 

.0753 

0.10850 

6.650' 

.0480 

0.06968 

4.672 

.0330 

0.04826 

4.001 

.0276 

0.04112 

1.372 

.0085 

0.01383 

(Barnes,  J.  phys.  Chem.  1898,  2.  545.) 

Sp.  gr.  of  Mg(NO3)2+Aq  at  20°  containing 
M  g.  mols.  of  salt  per  liter. 
M  0.02        0.05          0.10          0.15 

Sp.  gr.    1.00224  1.005626  1.011118  1.016557 

M  0.20        0.50          1.00          1.274 

Sp.  gr.  1.022026  1.054804  1.107865  1.136615 
(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38.  707.) 

'  Less  sol.  in  Ca(NO3)2+Aq  than  in  H2O. 
(Dijonval.) 

Very  easily  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  828.) 

+2H2O.  Mpt.  127°.  (Wasiljew,  C.  C. 
1909,  II.  1966.) 

+4H2O.    Mpt.  45.5°.    (W.) 

-f  6H2O.  Deliquescent.  Sol.  in  H2O  and 
alcohol.  Sol.  in  0.5  pt.  cold  H2O,  and  9  pts. 
cold  alcohol  of  0.84  sp.  gr.;  very  si.  sol.  in 
abs.  alcohol.  (Graham.) 

Melts  in  its  crystal  H2O  at  90°,  and  the  re- 
sulting liquid  boils  at  143.4°.  (Ordway,  Sill. 
Am.  J.  (2)  27.  14.) 

Solubility  in  H2O. 

Sat.  solution  contains  at: 
—18°      —4.5°        0°  18° 

38.03       39.50      39.96      42.33%  Mg(NO3)2, 

40°          80°  90°  (mpt.). 

45.87      53.69        57.81%  Mg(NO3)2. 
(Funk,  Z.  anorg.  1899,  20.  395.) 

+9H2O.    Solubility  in  H2O. 
Sat.  solution  contains  at: 

—23°      —20.5°      —18° 

35.44  36.19      38.03%  Mg(NO3)2. 

Cryohydrate  is  formed  at  — 29°.  (Funk, 
Z.  anorg.  1899,  20.  398.) 

Magnesium  neodymium  nitrate,  3Mg(NO3)2, 

2Nd(N03)3+24H20. 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  97.7  g.  hydrous  salt  at  16°. 
(Jantsch,  Z.  anorg.  1912,  76.  303.) 


Magnesium  praseodymium  nitrate, 

3Mg(NO3)2,  2Pr(NO3)3+24H2O. 
1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  7.70  g.  hydrous  salt  at  16°. 
(Jantsch.) 

Magnesium  samarium  nitrate,  3Mg(NO3)2. 

Sm(NO3)3-f-24H2O. 
(Demargay,  C.  R.  1900,  130.  1187.) 
1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 

1.325)  contains  24.55  g.  hydrous  salt  at  16°. 

(Jantsch.) 

Magnesium  thorium  nitrate,  MgTh(NO3)6-f- 

H2O. 

Hydroscopic;  sol.  in  HNO3.     (Meyer,  Z. 
anorg.  1901,  27.  385.) 

Magnesium    nitrate    ammonia,    Mg(NO3)2, 

6NH3. 

SI.  sol.  in  liquid  NH3.     (Franklin,  J.  Am. 
Chem.  Soc.  1913,  35.  1459.) 

Manganous  nitrate,   basic,   2MnO,   N2O5-h 

3H20. 
Sol.  in  H2O.    (Gorgeu.) 

Manganous  nitrate,  Mn(NO3)2. 

Deliquescent.      Easily    sol.    in    H2O    and 
alcohol. 

See  +3,  and  6H2O. 

Sp.  gr.  of  Mn(NO3)2+Aq  at  8°. 


%  Mn(NOs)2 
+6H2O 

Sp.  gr. 

%  Mn(N03)2 
+6H2O 

Sp.  gr. 

5 

1.0253 

45 

1.2705 

10 

1.0517 

50 

1.3074 

15 

1.0792 

55 

1.3459 

20 

1  .  1078 

60 

1.3861 

25 

1.1137 

65 

1.4281 

30 

1  .  1688 

70 

1.4721 

35 

1.2012 

71 

1.4811 

40 

1.2352 

(Oudemans,  Z.  anal.  7.  421.) 

Sp.  gr.  of  aqueous  solutions  containing: 
10          20  30    %  Mn(NO3)2+6H20, 

6.237     12.474     18.711%  Mn(NO3)2, 
1.052       1.107       1.165 

40  50  60    %  Mn(NO3)2+6H2O, 

24.948    31.185    37.422%  Mn(NO3)2, 
1.230      1.302      1.381 

70  80    %  Mn(NO3)2-f-6H2O. 

43.659    49.896%  Mn(NO3)2. 
1.466       1.558 

(Gerlach,  Z.  anal.  28.  477.) 

Sp.  gr.  of  Mn(NO3)2+Aq  at  room  temp, 
containing: 

18.309       29.602       49.309%  Mn(NO3)2. 
1.1482       1.3227       1.5056 

(Wagner,  W.  Ann.  1883,  18.  271.) 


NITRATE,  MERCURIC 


575 


Sp.  gr.  of  Mn(NO3)2+Aq  at  25°. 


Concentration  of 
Mn(NOs)2+Aq 


1-normal 


Sp.  gr. 


1.0690 
1.0349 
1.0174 
1.0093 


(Wagner,  Z.  phys.  Ch.  1890,  5.  39.) 

Sol.  in  liquid  NH3.  (Guntz,  Bull.  Soc 
1909,  (4)  6.  1006.) 

Very  sol.  in  liquid  NH3.  (Franklin,  Am 
Ch.  J.  1898,20.828.) 

+H2O.  Deliquescent.  (Guntz,  Bull.  Soc 
1909  (4)  5.  1005.) 

+3H2O.  From  solution  in  HNO3.  (Schultz- 
Sellack,  Zeit.  Ch.  1870.  646.) 

Solubility  in  H2O. 

Sat.  solution  contains  at: 
27°      29°      30°      34°     35.5°  mpt. 
65.66  66.99  67.38  71.31  76.82%  Mn(NO3)2. 
(Funk,  Z.  anorg.  1899,  20.  403.) 

+6H2O.  Melts  in  its  crystal  H2O  at  25.8° 
and  boils  at  129.4°.  (Ordway.) 

Solubility  in  H2O. 

Sat.  solution  contains  at: 
—29°  —26°  —21°  —16°   —5° 
42.29  43.15  44.30  45.52  48.88%  Mn(NO3)2, 

0°      +11°     18°    25.8°  mpt. 
50.49  54.50  57.33  62.37%  Mn(NO,)2. 

Cryohydrate  is  formed  at  — 36°.  (Funk, 
Z.  anorg.  1899,  20.  403.) 

Manganous  neodymium  nitrate,  3Mn(NO3)2, 

2Nd(N03)3+24H20. 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  296  g.  hydrous  salt  at  16°. 
(Jantsch,  Z.  anorg.  1912,  76.  303.) 

Manganous  praseodymium  nitrate, 

3Mn(NO3)2,  2Pr(NO3)3+24H2O. 
1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  23.4  g.  hydrous  salt  at  16°. 
(Jantsch.) 

Manganous  samarium  nitrate,  3Mn(NO3)2, 

2Sm(NO3)3+24H2O. 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  50.04  g.  hydrous  salt  at  16°. 
(Jantsch.) 

Manganous  thorium  nitrate,  MnTh(NO3)6-f- 

8H2O. 
Ppt.    (Meyer,  Z.  anorg.  1901,  27.  388.) 

Manganous  nitrate  cupric  oxide,  Mn(NO3)2, 

3CuO+3H2O. 
Ppt.    (Mailhe,  C.  R.  1902,  134.  234.) 


Manganous    nitrate    hydrazine,    Mn(NO3)2, 

2N2H4. 

Not  decomp.  by  H2O.  (Franzen,  Z.  anorg. 
1908,  60.  286.) 

Mercurous   nitrate,    basic,   2Hg2O,    N2Os+ 
H2O. 

Ppt.  Decomp.  by  boiling  with  H2O. 
(Marignac,  A.  ch.  (3)  27.  332.) 

Slowly  sol.  in  cold,  rapidly  in  hot  HCl+Aq: 
insol.  in  NH4C1,  and  NH4NO3+Aq. 

+  10H2O.  Slowly  sol.  in  normal  HNO3. 
(Reuss,  Dissert.  1886.) 

4Hg2O,  3N2O6+H2O.  Sol.  in  a  small  quan- 
tity of  H2O;  decomp.  by  a  large  amt.  of  H2O 
or  by  warm  H2O.  (Rose,  Pogg.  83.  154.) 

Is  3HgO,  2N2O5+H2O  according  to  Ger- 
hardt. 

+5H2O.    (Reuss,  Dissert.  1886.) 

5Hg2O,  3N2O5+2H2O.  (Marignac.)  Is 
2Hg2O,  N2O5+H2O.  (Lefort,  A.  56.  247.) 
Sol.  in  boiling,  less  sol.  in  cold  H2O.  (Marig- 
nac, L  c.) 

+4H2O,  and  +6H2O.  (Reuss,  Dissert. 
1886.) 

8Hg2O,  5N2O5+5H2O,  and  +11H2O. 
(Reuss.) 

HHg2O,  6N2O5+25H2O.    (Reuss.) 

16Hg2O,  9N2O6  +  19H2O,  +23H2O,  and 
+31H2O.  (Reuss.) 

3Hg2O,N2  O5+2H2O.  (Cox,  Z.  anorg.  1904, 
40.  177.) 

Mercurous  nitrate,  HgNO3. 

Very  sol.  in  liquid  NH3.  (Franklin,  Am. 
Ch.  J.  1898,  20.  829.) 

Fairly  sol.  in  boiling  CS2.  (Arctowski,  Z. 
anorg.  1894,  6.  257.) 

SI.  sol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1369.) 

Sol.  in  methylamine.  (Franklin, "  J.  Am. 
Chem.  Soc.  1906,  28.  1419.) 

+H2O.  Completely  sol.  in  a  little  warm 
H2O,  but  decomp.  by  more  H2O.  Completely 
sol.  as  acid  salt  in  H2O  containing  HNO3. 
(Marignac,  A.  ch.  (3)  27.  332.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

+1V4H20,  +1V.HA  +W2H20,  etc. 
(Reuss,  Dissert.  1896.) 

Mercuric  nitrate,  basic,  6HgO,  N2O5  (?). 

Insol.  in  hot  H2O.    (Kane.) 

3HgO,  N2O5+H2O.  Decomp.  to  oxide  by 
washing  with  cold  H2O.  Sol.  in  dil.  HNO3  + 
Aq.  (Millon,  A.  ch.  (3)  18.  361.) 

2HgO,  N2O5+H2O.  SI.  deliquescent.  De- 
comp. by  H2O;  sol.  in  dil.  HNO3+Aq. 
Millon.) 

+2H2O.  Decomp.  by  cold  H2O.  Deli- 
quescent. Sol.  in  H2O  containing  HNO3. 
(Marignac.) 

+3H2O.    (Ditte,  J.  B.  1854.  366.) 

Mercuric  nitrate,  Hg(NO3)2. 
Very  sol.  in  liquid  NH3.     (Franklin,  Am. 
h.  J.  1898,  20.  829.) 


576 


NITRATE,  MERCUROMERCURIC 


Neither  dissolved  nor  attacked  by  liquid 
NO2.  (Frankland,  Chem.  Soc.  1901,  79. 
1361.) 

Sol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1369.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

Difficultly  sol.  in  ethyl  acetate.  (Naumann, 
B.  1910,  43^.  314.) 

Sol.  in  methylal.  (Eidmann,  C.  C.  1899. 
II,  1014.) 

+  MH2O.  Deliquescent.  Very  sol.  in  a 
little  H2O.  H2O  precipitates  basic  salt  from 
cone.  Hg(NO3)2+Aq.  Insol.  in  alcohol. 
Decomp.  by  ether.  (Millon.) 

+H2O.  Extraordinarily  sol.  in  H2O. 
(Cox,  Z.  anorg.  1904,  40.  159.) 

+8H2O.  Melts  at  6°  in  crystal  H2O. 
(Ditte.) 

Mercuromercuric  nitrate,  Hg2O,  2HgO,  N2O5. 

Boiling  H2O  gradually  dissolves  out 
Hg2(NO3)2,  and  leaves  residue  of  HgO  and 
Hg. '  (Brooks,  Pogg.  66.  63.) 

2Hg2O,  HgO,  N2O6+H2O.  (Ray,  Chem. 
Soc.  1905,  87.  175.) 

Hg20,  2HgO,  N205+H20.    (Ray.) 

Mercurous  hydrogen  nitrate,  4HgNO3,  HNO3 

+8H2O. 

(Reuss,  Dissert.  1886.) 
5HgNO3,  3HNO3+26H2O.    (Reuss.) 

Mercuric  silver  nitrate,  Hg(NO3)2,  2AgNO3. 
Easily  sol.  in  H2O  without  decomp.    (Ber- 
zelius.)* 

Mercurous  strontium  nitrate,  2SrO,  2Hg2O, 
3N205. 

Decomp.  by  H2O.  Much  more  sol.  in  H2O 
than  the  corresponding  Ba  compound. 

Readily  sol.  in  warm  dil.  HNO3+Aq  or 
Hg2(NO3)2+Aq  without  decomposition. 
(Stadeler,  A.  87.  131.) 

Mercurous  thallous  nitrate,  HgNO3,  T1NO3. 

Miscible  with  H2O.  (Retgers,  N.  Jahrb. 
Miner,  1896.  II,  183.) 

Mercuric  nitrate  bromide,  Hg(NO3)2,  HgBr2. 
(Morse,  Z.  phys.  Ch.  1902,  41.  733.) 

Mercuric  nitrate  cadmium  oxide,  Hg(NO3)2, 

CdO+2H2O. 

Ppt.    (Mailhe,  Bull.  Soc.  1901,  (3)  26.  788.) 
+3H2O.    Decomp.  by  H2O.    (Mailhe.) 

Mercuric  nitrate  cobaltous  oxide,  Hg(NO3)2, 

CoO+3H2O. 

Ppt,  '  (Mailhe,  C.  R.  1901,  132.  1275.) 
+4H2O.    Decomp.  by  H2O.     (Mailhe,  A. 

ch.  1902,  (7)  27.  369.) 


Mercuric   nitrate    cupric    oxide,    Hg(N03)2, 

CuO+2H2O,  and  +4H2O. 
(Mailhe,  Bull.  Soc.  1901,  (3)  25.  791.) 
+5H2O.     Decomp.  by  H2O.     (Mailhe,  A. 

ch.  1902,  (7)  27.  365.)    ' 

Mercuric  nitrate  cyanide,  Hg(NO3)2, 

Hg(CN)2. 

Very  sol.  in  H2O.  Very  sol.  in  methyl  al- 
cohol and  solution  is  not  decomp.  at  bpt. 
Ethyl  alcohol  apparently  decomp.  it.  (Prus- 
sia, Gazz.  ch.  it.  1898,  28.  (2)  115.) 

Mercurous  nitrate  hydrazine,  2HgNO3,  N2H4. 

Decomp.  by  H2O.  Stable  in  dil.  HNO3+ 
Aq  solution.  (Hofmann  and  Marburg,  A. 
1899,  305.  215.) 

Ppt.;  very  unstable.  (Hofmann,  B.  1897, 
30.2021.) 

Hg(NO3)2,  N2H4.  Sol.  in  dil.  HC1  and 
HNO3.  (Hofmann  and  Marburg,  A.  1899, 
305.  215.) 

Ppt.;  sol.  in  acids;  decomp.  by  alkali. 
(Hofmann,  B.  1897,  30.  2021.) 

Mercuric  nitrate  iodide,  Hg(NO3)2,  2HgI2. 

Decomp.  by  long  boiling  with  H2O.  (Rie- 
gel,  Jahrb.  Pharm.  11.  396.) 

2Hg(NO3)2,  3HgI2.  Easily  decomp.  by 
H2O ;  less  easily  by  alcohol  or  ether.  (Riegel.) 

Hg(NO3)2,  HgI2.  Decomp.  very  quickly 
by  HNO3+Aq  or  alcohol  of  0.814  sp.  gr. 
(Souville,  J.  Pharm.  26.  474.) 

Mercuric  nitrate  manganous  oxide,  Hg(NO3)2, 
MnO+2H2O. 

Decomp.  by  H2O.  (Mailhe,  Bull.  Soc. 
1901,  (3)  26.  790.) 

+3H2O.    (Mailhe.) 

+4H2O.  (Mailhe,  A.  ch.  1902,  (7)  27. 
370.) 

Mercuric  nitrate  nickel  oxide,  Hg(NO3)2,  NiO 
+2H2O. 

(Mailhe,  Bull.  Soc.  1901,  (3)  25.  788.) 
+4H2O.    Decomp.  by  H2O.     (Mailhe,  A. 
ch.  1902,  (7)  27.  369.) 

Mercurous    nitrate    phosphate,    HgNO3, 
Hg3P04+H20. 

Insol.  in  H?O,  but  decomp.  by  boiling  there- 
with. Insol.  in  H3PO4+Aq  or  alcohol.  Com- 
pletely sol.  in  hot  NH4Cl-hAq.  Decomp.  by 
cold  KOH+Aq,  and  warm  K2CO3+Aq. 
(Wittstein.) 

2HgNO3,  Hg,O,  5Hg3PO4+H2O.  (Haack, 
A.  262.  192.) 

Mercuric  nitrate  silver  bromide,  Hg(NO3)2, 

AgBr. 
(Morse,  Z.  phys.  Ch.  1902,  41.  733.) 


NITRATE,  NICKEL 


577 


Mercuric     nitrate     silver     cyanide,     basic, 

Hg(OH)NO3,  AgCN+2H2O. 
'    (Schmidt,  Z.  anorg.  1895,  9.  431.) 

Hg(OH)NO3,  .    5Ag2O,     20AgCN+7H2O. 
(Schmidt.) 

^VTercuric   nitrate    silver   iodide,   Hg(N03)2, 


Decomp.  by  H2O.    (Preuss,  A.  29.  328.) 

Mercuric  nitrate  sulphide,  Hg(NO3)2,  2HgS. 

Very  si.  sol.  in  hot  H2O.  Insol.  in  HNO3+ 
Aq.  Decomp.  by  hot  H2SO4  or  aqua  regia, 
also  by  hot  HCl+Aq.  (Barfoed,  J.  pr.  93. 
230.) 

Sol.  in  aqua  regia.  (Deniges,  Bull.  Soc. 
1915,  (4)  17.  355.) 

2Hg(N03)2JftgO,  6HgS+12H20.  Insol. 
in  H2O,  and  IW"O3+Aq  of  1.2  sp.  gr.  (Gramp, 
J.  pr.  (2)  14.  299.) 

Mercuric  nitrate  zinc  oxide,  Hg(NO3)2,  ZnO-f 

H20. 

Ppt.  Decomp.  by  H2O.  (Mailhe,  C.  R. 
1901,  132.  1274.) 

Molybdenum  nitrate,  Mo2O3,  N2O6  (?). 
Sol.  in  dil.  HNO3+Aq.  (Berzelius.) 
MoO2,  2N2O5  (?).  Sol.  in  dil.  HNO3+Aq. 

(Berzelius.) 

Neodymium  nickel  nitrate,  2Nd(N08)3, 

3Ni(NO3)2+24H2O. 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  116.6  g.  hydrous  salt  at  16°. 
(Jantsch,  Z.  anorg.  1912,  76.  303.) 

Neodymium  rubidium  nitrate,  [Nd(NO3)5]Rb2 

+4H2O. 

Hydroscopic.  (Jantsch,  Z.  anorg.  1911, 
69.  230.) 

Neodymium  zinc  nitrate,  2Nd(NO3)3, 

3Zn(NO3)2+24H2O. 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  177  g.  hydrous  salt  at  16°. 
(Jantsch.) 

Nickel  nitrate,  basic. 

Insol.  in  H2O.    (Proust.) 

8NiO,  2N2O6+5H2O.  Insol.  in  cold  or  hot 
H2O.  (Habermann,  M.  5.  432.) 

5NiO,  N2O5+4H2O.  Not  decomp.  by  boil- 
ing H2O.  (Rousseau  and  Tite,  C.  R.  114. 
1184.) 

Nickel  nitrate,  Ni(NO3)2. 

Solubility  in  H2O.    See  +3,  6,  and  9H2O. 

Sp.  gr.  of  aqueous  solution  at  17.5°  contain- 
ing: 

5  10  15  20  %Ni(NO3)2, 

1.0463  1.0903  1.1375  1.1935 

25  30  35  40     %  Ni(NO8)2. 

1.2534     1.3193     1.3896     1.4667 

(Franz,  J.  pr.  (2)  6.  295.) 


91.5 g.(  = 
1.073 


Sp.    gr.    of    Ni(NO,;_  . 
Ni(NO3)2  (anhydrous)   in   1000  g.   H2O  at 
24.4°:    ' 

ol.)  183  274.5    369  460.5  549 
1.141  1.205  1.266  1.324  1.378 
(Gerlach,  Z.  anal.  28.  468.) 

Sp.  gr.  of  Ni(NO3)2+Aq  at  room  temp, 
containing: 

16.493      30.006      40.953%  Ni(NO8)2. 
1.1363      1.2776      1.3879 

(Wagner,  W.  Ann.  1883,  18.  269.) 

Sp.  gr.  of  Ni(N03)2+Aq  at  25°. 


Concentration  of 
Ni(NO3)2+Aq 

Sp.  gr. 

1-normal 

Vr-      " 

1U-     " 

Vs-       " 

1.0755 
1.0381 
1.0192 
1.0096 

(Wagner,  Z.  phys.  Ch.  1890,  5.  39.) 

Sp.  gr.  at  20°  of  Ni(NO3)2+Aq  containing 
M  g.  mols.  of  salt  per  liter. 
M         0.01          0.025        0.05          0.075 
Sp.  gr.  1.001521  1.003882  1.007792  1.011541 

M         0.1  0.25          0.5  0.75 

Sp.  gr.  1.015307  1.03837     1.07611     1.11310 

M         1.0  1.5  2.0 

Sp.  gr.  1.14562     1.22134     1.29459 

(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38.  720.) 

Sol.  in  liquid  NH3.     (Guntz,   Bull.  Soc. 
1909.  (4)  6.  1008.) 

Moderately  sol.  in  liquid  NH3.    (Franklin, 
Am.  Ch.  J.  1898,  20.  828.) 

Solubility  in  glycol  =  7.5%.     (de  Coninck, 
C.  C.  1905,  II.  1234.) 

Insol.  in  benzonitrile.    (Naumann,  B.  1914, 
47.  1370.) 

+3H2O.    Solubility  in  H2O. 

Sat.  solution  contains  at: 
58°       60°       64°        70° 

61.61     61.99    62.76    63.95%  Ni(NO3)2, 

90°       95°  mpt. 
70.16    77.12%  Ni(N03)2. 

(Funk,  Z.  anorg.  1899,  20.  411.) 

+6H2O.    Not  deliquescent  in  dry  ah*.    Sol. 
in  2  pts.  cold  H2O  and  in  alcohol.    (Tupputi.) 

Mpt.  of  Ni(NO3)2+6H2O=56.7°.     (Ord- 
way;  Tilden.  Chem.  Soc.  46.  409.) 

Sat.  solution  boils  at  136.7°.    (Ordway.) 

Solubility  in  H2O. 

Sat.  solution  contains  at: 
—21°     —12.5°     —10°       —6° 
39.94         41.59     42.11      43.00%  Ni(NO8)2, 


0°          +20°        41°        56.7°  mpt. 
44.32       49.06       55.22      62.76%  Ni(N03)2. 
(Funk,  Z.  anorg.  1899,  20.  410.) 


578 


NITRATE,  NICKEL  PRASEODYMIUM 


Sat.  solution  of  Ni(NO3)2+6H2O  contains 
44.3%  Ni(N08)2  at  0°,  and  48.7%  Ni(NO3) 
at  18°.    (Mylius,  Z.  anorg.  1912,  74.  411.) 

Sp.  gr.  of  Ni(NO3)2+Aq  containing  in  1000 
g.  H2O  at  24.4°,  g.  Ni(NO3)2+6H2O. 
145.5  g.  (  =  H  mol.)  291      436.5      582 
1.069  1.128     1.179     1.224 

727.5         873       1018.5       1164 

1.264       1.299       1.329       1.357 

(Gerlach,  Z.  anal.  28.  468.) 

•Sol.  in  NH4OH+Aq. 

Insol.  in  absolute  alcohol. 

SI.  sol.  in  acetone.    (Krug  and  M'Elroy.) 

Difficultly  sol.  in  methyl  acetate.  (Nau- 
mann,  B.  1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

+9H2O.    Solubility  in  H2O. 

Sat.  solution  contains  at: 
—23°      —21°      —10.5° 
39.02       39.48          44.13%  Ni(N03)2. 

Cryohydrate  is  formed  at  —  27°.  (Funk, 
Z.  anorg.  1899,  20.  411.) 

Nickel    praseodymium    nitrate,    3Ni(NO3)2, 
2Pr(NO3)3+24H2O. 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  9.28  g.  hydrous  salt  at  16°. 
(Jantsch,  Z.  anorg.  1912,  76.  303.) 

Nickel  samarium  nitrate,  3Ni(NO3)2, 

2Sm(NO3)3+24H2O. 

1  1.  sat.  solution  in  HNO8+Aq  (sp.  gr. 
1.325)  contains  29.11  g.  hydrous  salt  at  16°. 
(Jantsch.) 

Nickel  thorium  nitrate,  NiTh(N03)6+8H2O. 
Sol.   in  HN03+Aq.     (Meyer,   Z.   anorg. 
1901,  27.  387.) 

Nickel  uranyl  nitrate,  10Ni(NO3)2, 

3(U02)(N03)2. 

Sol.  in  H2O  and  acids;  insol.  in  aq.  alkali. 
(Lancien,  C.  C.  1912,  1.  208.) 

Nickel  nitrate  ammonia,  Ni(NO3)2,  4NH3+ 

2H20. 

Efflorescent.  Easily  sol.  in  cold  H2O; 
decomp.  by  boiling.  Insol.  in  alcohol. 
(Erdmann,  J.  pr.  97.  395;  Ephraim,  B.  1913, 
46.  3106.) 

.    (Andre,  C.  R.  106.  936.) 


Nickel  nitrate  chloride  ammonia,  6Ni(NO3)2, 

NiCl2,  30NH3+16H2O. 
Sol.  in  H20  with  decomp.     (Schwarz,  W. 
A.  B.  1850.  272.) 

Nickel  nitrate  cupric  oxide,  Ni(NO3)2,  3CuO-f 

3H20. 
Ppt.    (Maihle,  C.  R.  1902,  134.  234.) 


Nickel  nitrate  hydrazine,  Ni(NO3)2,  3N2H4. 

Insol.  in  H2O.  Decomp.  by  hot  H2O. 
Easily  sol.  in  dil.  acids.  (Franzen.  Z.  anorg. 
1908,  60.  267.) 

Palladium  nitrate,   basic,   Pd(NO3)2,   3PdO 
+4H20. 

Ppt.    Insol.  in  H2O.    (Kane.) 
Palladium  nitrate,  Pd(NO3)2+zH2O. 

Very  deliquescent,  and  sol.  in  H2O.  De- 
comp. by  much  H2O  or  alcohol.  (Kane.) 

Decomp.  by  cold  or  hot  H2O.  (Rose,  A.  83. 
143.) 

Platinic  nitrate,  Pt(NO3)4  (?). 

Known  only  in  solution,  which  is  decomp. 
on  evaporating.  (Berzelius.) 

Pt(NO3)2,  3PtO2+5H2O.  Insol.  in  H20. 
(Prost,  Bull.  Soc.  (2)  46.  156.) 

Platinum  nitrate  sulphocarbamide.  Pt(NO3)2, 

4CS(NH2)2. 

Very  sol.  in  H2O.  Unstable.  (Kurnokow, 
J.  pr.  1894,  (2)  50.  490.) 

Potassium  nitrate,  KNO3. 

Not  deliquescent,  but,  according  to  Mulder, 
100  pts.  KNO3  under  a  bell  jar  with  H2O  take 
up  339  pts.  H2O  in  22  days,  and  small  amounts 
finally  deliquesce  completely. 

Sol.  in  H2O  with  absorption  of  heat. 

16  pts.  KNO3  +  100  pts.  H2O  at  13.2°  lower 
the  temperature  10.2°.  If  the  initial  temp,  is 
23°  it  falls  to  12.8°,  if  0°  it  does  not  fall  below 
— 2.7°,  which  is  the  freezing-point  of  the 
mixture.  (Riidorff,  Pogg.  136.  276.) 

KNOa+Aq  sat.  at  18.1°  has  1.1601  sp.  gr.  and  con- 
tains 22.72%  KNOa,  or  100  pts.  H2O  at  18.1°  dissolve 
29.45  pts.  KNOa.  (Karsten,  1840.) 

Sol.  in  3.745  pts.  H2O  at  15°.     (Gerlach.) 

Sol.  in  3  pts.  HzO  at  21°  (Schiff,  A.  109.  326),  and 
solution  has  1.1683  sp.  gr. 

Sol.  in  3  pts.  cold,  and  0.5  pt.  boiling  H2O.  (Four- 
croy.) 

KNOs+Aq  sat.  at  18°  has  sp.  gr.  1.151,  and  contains 
21.63%  KNOa,  or  100  pts.  H2O  dissolve  27.60  pts. 
KNOa  at  18°.  (Longchamp.) 

Sol.  in  4  pts.  H2O  at  16°,  and  0.25  pt.  at  b.-pt.  (Rif- 
fault.) 

100  pts.  H2O  at  114.5°  dissolve  284.61  pts.    (Griffiths.) 

Sol.  in  7  pts.  cold,  and  1  pt.  boiling  H2O.  (Berg- 
mann.) 

Sol.  in  6.15  pts.  cold  H2O  at  18.75°.     (Abl.) 

100  pts.  H2O  at  15.5°  dissolve  26.6  pts.;  at  100°,  100 
pts.  (Ure's  Dictionary.) 

KNOa+Aq  sat.  at  10°  contains  33.3%.     (Eller.) 

KNOa+Aq  sat.  in  the  cold  contains  25%.  (Four- 
croy.) 

KNOa+Aq  sat.  at  12.5°  contains  24.8%.  (Hassen- 
fratz.) 

Solubility  of  KNO3  in  100  pts.  H2O  at  t°. 


t 

Pts.  KNOa 

t° 

Pts.  KNO» 

0 
5 
11.67 
17.91 
24.94 

13.2 
16.7 
22.2 
29.3 

38.4 

45.10 
54.72 
65.45 
79.72 
97.66 

74.7 
97.1 
125.5 
169.2 
236.4 

(Gay-Lussac,  A.  ch.  11.  314.) 

NITRATE,  POTASSIUM 


579 


Solubility  of  KNO3  in  100  pts.  H2O  at  t°. 


t° 

Pts.  KNOs 

16.0 
29 
44.2 

26.7 
43.5 
71.4 

(Nordenskjold,  Pogg.  136.  312.) 

100  pts.  H2O  dissolve  at: 
10°       18°       27°        41°        53° 
21.2      27.9      40.1      66.3      93.3  pts.  KNO3. 
(Gerardin,  A.  ch.  (4)  6.  150.) 

100  pts.  KNO3+Aq  sat.  at  14°  contain 
16.34  pts.  KNO3;  at  15°,  18.81  pts.  KNO3. 
(v.  Hauer,  J.  pr.  98.  177.) 

100  pts.  H2O  dissolve  at: 
4°         16.3°        68.3° 
16        27.2          132.1  pts.  KNO3. 
(Andreae,  J.  pr.  (2)  29.  456.) 

Solubility  in  100  pts.  H2O  at  t°. 


t° 

Pts 
KNOs 

t° 

Pts. 
KNOs 

t° 

Pts. 
KNOs 

0 

13.3 

39 

62 

78 

165 

1 

13.8 

40 

64 

79 

168 

2 

14.6 

41 

66 

80 

172 

3 

15.5 

42 

68 

81 

175 

4 

16.4 

43 

70 

82 

179 

5 

17.1 

44 

72 

83 

182 

6 

17.8 

45 

74 

84 

185 

7 

18.5 

46 

76 

85 

189 

8 

19.3 

47 

78 

86 

192 

9 

20.2 

48 

81 

87 

196 

10 

21.1 

49 

83 

88 

199 

11 

22.0 

50 

86 

89 

203 

12 

23.0 

51 

88 

90 

206 

13 

24.0 

52 

91 

91 

210 

14 

25.0 

53 

93 

92 

214 

15 

26.0 

54 

96 

93 

218 

16 

27.0 

55 

98 

94 

222 

17 

28.1 

56 

101 

95 

226 

18 

29.1 

57 

103 

96 

230 

19 

30.2 

58 

106 

97 

234 

20 

31.2 

59 

108 

98 

238 

21 

32.3 

60 

111 

99 

243 

22 

33.5 

61 

113 

100 

247 

23 

34.7 

62 

116 

101 

252 

24 

36.0 

63 

119 

102 

256 

25 

37.3 

64 

121 

103 

261 

26 

38.6 

65 

124 

104 

266 

27 

40.0 

66 

127 

105 

272 

28 

41.4 

67 

130 

106 

278 

29 

42.9 

68 

133 

107 

284 

30 

44.5 

69 

136 

108 

289 

31 

46.0 

70 

139 

109 

295 

32 

48 

71 

142 

110 

301 

33 

50 

72 

146 

111 

307 

34 

52 

73 

149 

112 

313 

35 

54 

74 

152 

113 

319 

36 

56 

75 

155 

114 

326 

37 

58 

76 

159 

114.1 

327.4 

38 

60 

77 

162 

(Mulder,  Scheik.  Verhandel.  1864.  89.) 


100  pts.  H2O  dissolve  493  pts.  KNO3  at 
125°.  (Tilden  and  Shenstone,  Phil.  Trans. 
1884.  23.) 

Rhombohedral  KNO3  is  more  easily  soluble 
than  the  prismatic,  and  easily  forms  super- 
saturated solutions.  (Frankenheim.) 

Sat.  KNO3+Aq  contains  at: 

139°     158°     160°     175°     180° 

79.8     83.7     83.9     84.0     84.2%  KNO3. 

190°    215°    225°    258°    283° 
86.0     89.0     90.4     91.6     96.5%  KNO3. 
(fitard,  A.  ch.  1894,  (7)  2.  526.) 

Solubility  in  100  pts.  H20  at  t°. 


t° 

G.  KN03 

0.40 

13.43 

14.90 

25.78 

30.80 

47.52 

44.75 

74.50 

60.05 

111.18 

76 

156.61 

91.65 

210.20 

114* 

311.64 

Sp.  gr.t°/4e 


1.0817 
1 . 1389 
1.2218 
1.3043 
1.3903 
1.4700 
1.5394 
1.6269 


*  B.-pt.  of  sat.  solution. 
(Berkeley,  Phil.  Trans.  1904,  203,  A,  189.) 

100  g.  H2O  dissolve  37.79  g.  KNO3  at  25°. 

100  g.  H2O  dissolve  3.08  g.  equiv.  KNO3 
at  20°;  3.27  at  21.5°.  (Euler,  Z.  phys.  Ch. 
1904,  49.  312.) 

1  1.  H2O  dissolves  384.48  g.  KNO3  at  25°. 
(Armstrong  and  Eyre,  Proc.  Roy.  Soc.  1910, 
A,  84.  123.) 

1  1.  sat.  KNOs+Aq  contains  2.8  g.  mols. 
KNO3.  (Rosenheim  and  Weinheber,  Z. 
anorg.  1911,  69.  263.) 

100  g.  H2O  dissolve  38.485  g.  KNO3  at  25°. 
(Haigh,  J.  Am.  Chem.  Soc.  1912,  34.  1148.) 

Sat.  KNO3+Aq  contains  at: 
50°  58°  62°  68° 

46.39        51.55        53.64        57.04%  KNO3. 
(Tschugaeff,  Z.  anorg.  1914,  86.  160.) 

Solubility  in  H2O. 

100  g.  of  the  sat.  solution  contain  at: 
9.1°        21.1°          35° 
16.76       24.77       35.01  g.  KNO3. 
(Findlay,  Chem.  Soc.  1914,  105.  780.) 

Sp.  gr.  of  solution  sat.  at  15°  =  1.134. 
(Michel  and  Krafft.) 

Sp.  gr.  of  solution  sat.  at  16°  =  1.138. 
(Stolba,  J.  pr.  97.  503.) 

Sp.  gr.  of  solution  sat.  at  18°  =  1.1601,  and 
contains  29.45%  KNO3.  (Karsten.) 

Sp.  gr.  of  KNO3+Aq  at  19.5°. 


%  KNOs 

Sp.  gr. 

%  KNOs 

.     Sp.  gr. 

4.871 
9.618 
14.044 

1.0307 
1.0618 
1.0920 

17.965 

21.488 

1.1198 
1.1457 

(Kremers,  Pogg.  95.  120.) 


580 


NITRATE,  POTASSIUM 


Sp.  gr.  of  KNO3+Aq  at  21°. 

Sp.  gr.  of  KNO3+Aq 

at  25°. 

%  KNOs 

Sp.  gr. 

%  KNOs 

Sp.  gr. 

Concentration  of 
KNOs+Aq. 

Sp.  gr.      ^ 

1 

2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 

1.0058 
1.0118 
1.0178 
.0239 
.0300 
.0363 
.0425 
.0490 
.0555 
.0621 
.0686 
1.0752 

13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 

1 
1 
1 
1 
1 
1 
1 
1 
1 
1 
1 
1 

.0819 
.0887 
.0956 
.1026 
.1097 
.1169 
.1242 
.1316 
.1390 
.1464 
.1538 
.1613 

1-normal 

I/*-   ;; 

1.0605 
1.0305 
1.0161 
1.0075 

(Wagner, 

Sp.  gr.  ( 

p  =  per  cent 
served  density 

percc-(l55=1 

Z.  phys.  Ch.  18 

)f  KNO3+Aqa 
strength  of  sc 

90,  5.  37.) 

t  20.1°. 

Jution;  d=ob- 
;onc.  in  grams 

(Schiff,  A.  110.  75.) 
Sp.  gr.  of  KNO3+Aq  at  15°. 

%  KNOs 

Sp.  gr. 

%  KNOs 

Sp.  gr. 

P 

d 

w 

1 

2 
3 

4 
5 
6 
7 
8 
9 
10 
11 

.00641 
.01283 
.01924 
.02566 
.03207 
.03870 
.04534 
.05197 
.05861 
.06524 
.07215 

12 
13 
14 
15 
16 
17 
18 
19 
20 
21 

1. 
1. 
1. 
1. 
1. 
1. 
1. 
1. 
1. 
1. 

07905 
08596 
09286 
09977 
10701 
11426 
12150 
12875 
13599 
14361 

25.54 
21.95 

17.88 
13.93 
8.706 
5.393 
4.389 
2.848 
2.030 
0.741 

1  .  1783 
1.1510 
1.1200 
1.0913 
1.0553 
1.0331 
1.0264 
1.0165 
1.0113 
1.0030 

0.30095 
0.25270 
0.20033 
0.15203 
0.09186 
0.05571 
0.04506 
0.02895 
0.02053 
0.00743 

(Gerlach,  Z.  anal.  8.  286.) 
Sp.  gr.  of  KNO3+Aq  at  17.5°. 

(Barnes,  J.  Phys.  Chem.  1898,  2.  544.) 

Sp.  gr.  20°/4°  of  a  normal  solution  of  KN03 
=  1.05954;  of  a  0.5  normal  solution  =  1.029325. 
(Haigh,  J.  Am.  Chem.  Soc.  1912,  34.  1151.) 

Sp.  gr.  of  sat.  KNO3+Aq  at  t°. 

KN^bs     SP-^'       KNOs 

Sp.  gr.       K^0j 

Sp.  gr. 

1   .    1.006          8 
2         .012         9 
3         .019        10 
4         .025        11 
5         .032        12 
6         .038        13 
7         .045        14 

1.051        15 
1.058        16 
1.065        17 
1.072        18 
1.078        19 
1.085        20 
1.092 

1.099 
1.106 
1.113 
1.120 
1.127 
1.134 

t° 

G.  KNOs  sol.  in 
100  g.  H20 

Sp.  gr. 

G 
10 
20 
30 
40 
50 
60 
70 

13.27 
20.89 
31.59 
45.85 
63.90 
85.51 
109.00 
138.00 

.084 
.120 
.161 
.212 
.282 
.339 
.403 
1.446 

(Hager,  Comm.  1883.) 
Sp.  gr.  of  KNO3+Aq  at  18°. 

%  KNOs 

Sp.  gr. 

^  %  KNOs 

Sp.  gr. 

5 
10 
15 

1.0305 
1  .  0632 
1.097 

20 

22 

1.133 

1.148 

(Kohlrausch,  W.  Ann.  1879.  1.) 

Sp.  gr.  of  KNO3+Aq  at  20°,  containing  mols. 
KNO3  in  100  mols.  H2O. 

(Tschernaj,  J.  Russ.  Phys.  Chem.  Soc.  1912, 
44.  1565.) 

The  saturated  solution  boils  at  114.1°  (Mul- 
der); 114.5°  (Griffiths);  115.9°  (Legrand,  Ger- 
ardin);  117°  (Magnus);  118°  (Kremers);  126° 
(Le  Page). 
The  saturated  solution  forms  a  crust  at 
111°,  and  boils  at  115°;  highest  temp,  ob- 
served, 115.3°.    (Gerlach,  Z.  anal.  26.  426.) 

Mols. 
KNOs 

Sp.  gr. 

Mols. 
KNOs 

Sp.  gr. 

0.5 
1 

2 

1.01730 
1.03373 
1.06524 

4 
5 

1 
1 

.  12264 

.  14888 

(Nicol,  Phil.  Mag.  (5)  16.  122.) 

NITRATE,  POTASSIUM 


581 


B.-pt  of  KNO+Aq  containing  pts.  KNO3  to 
100  pts.  H2O.  G  =  according  to  Gerlach 
(Z.  anal.  26.  444);  L  =  according  to 
Legrand  (A.  ch.  (2)  62.  426). 


B.-pt. 

G 

L 

B.-pt. 

G 

L 

100.5° 

7.5 

107° 

120.5 

119.0 

101 

15.2 

i2.'2 

108 

141.5 

140.6 

101.5 

23 

109 

164 

163.0 

102 

31 

26\4 

110 

188.5 

185.9 

102.5 

39 

111 

215 

209.2 

103 

47.5 

42^2 

112 

243 

233.0 

103.5 

56 

113 

274 

257.6 

104 

64.5 

5<K6 

114 

306 

283.3 

104.5 

73 

115 

338.5 

310.2 

105 

82 

78,3 

115.9 

335.1 

106 

101 

98.2 

... 

... 

1  pt.  KNO3  dissolves  in  £.4  pts.  HNO3;  at 
20°  in  3.8  pts.,  and  at  123°  in  1  pt.  HNO3+Aq 
of  1.423  sp.  gr.  (Composition  2HNO3,  3H2O.) 
(Schultz,  Zeit.  Ch.  (2)  5.  531.) 

Solubility  of  KNO3  in  HN03  at  0°. 


G.  per  100  cc.  solution 

Sp.  gr. 

KNOs 

HNOs 

12.65 

0.00 

1.079 

10.02 

3.71 

8.38 

8.38 

1^093 

7.49 

13.58 

1.117 

7.49 

19.47 

1.144 

7.68 

30.04 

1.202 

10.42 

42.86 

1.289 

28.64 

75.95 

1.498 

(Engel,  C.  R.,  1887,  104.  913.) 
Solubility  in  ANO3+Aq. 


Solution 
temp. 


+14.0 
17.0 
19.5 
22.0 
21.5 
21.5 
20.0 
—  4.0 
+16.5 
22.5 
23.5 
25.5 
27.0 
29.0 
30.5 
21.0 
39.0 
50.0 


24.4 

32.6 
34.8 
37.2 
44.5 
47.8 
48.6 
50.9 
37.2 
44.5 
47.2 
47.8 
48.6 
49.4 
50.1 
50.9 
49.4 
50.9 
51.7 


Solid  phase 


KNO3,  2HNO3(solution  in 
HNO3)  (stable) 


(mpt.) 
(Solution  in  KNO3)  (labile) 


KNO3,  HNO3  (labile) 
(stable) 

a 
(t 

(labile) 

KNOs(labile) 

(stable) 


Sol.  in  sat.  NH4Cl+Aq.  Solution  thus 
obtained  contains  43.07  pts.  mixed  salts,  or 
100  pts.  H2O  dissolve  75.66  pts.  mixed  salts, 
viz.  38.62  pts.  KNO3  and  39.84  pts.  NH4C1. 
(Karsten.)  See  also  under  NH4C1. 

Solubility  of  KNO3+K2CO3  and  KHCO3 
in  H2O,  see  under  K2CO3  and  KHCO3. 

Sol.  in  sat.  BaCl2+Aq  with  pptn.  of 
Ba(N03)2. 

Sol.  in  sat.  NH4NO3+Aq,  at  first  without 
pptn.,  but  afterwards  NH4NO3  is  pptd.  (Kar- 
sten.) 

Sol.  in  NH4NO3+Aq  with  pptn.  of 
NH4NO3.  (Riidorff,  B.  6.  485.) 

See  also  under  NH4NO3. 

Sol.  in  sat.  Ba(NO3)2+Aq,  but  soon  a 
double  salt  separates.  (Karsten.) 

See  also  under  Ba(NO3)2. 

Sol.  in  Ca(NO3)2+Aq.    (Longchamp.) 

See  also  under  Ca(NO3)2. 

Sol.  in  sat.  Pb(NO3)2+Aq  without  pptn. 

100  pts.  H2O  dissolve  119.6  pts.  Pb(NO3)2 
and  67.1  pts.  KNO3  at  21.2°.  (Riidorff,  B.  6. 
484.)  See  also  under  Pb(NO3)2. 

Solubility  in  AgNO3+Aq  at  t°. 


t° 

Sat.  solution  contains 

%  KNOs 

%  AgNOa 

%  total  salt 

7 

10.5 

39.4 

49.9 

—7.5 

10.5 

40.5 

51.0 

—4 

11.3 

42.5 

53.8 

+20 

23.6 

46.4 

70.0 

33 

26.3 

50.9 

77.2 

34 

27.3 

51.1 

78.4 

36 

29.4 

52.0 

81.4 

38 

81.7 

46 

82.3 

54 

33]  1 

55.0 

88.1 

54 

55.8 

61 

89^5 

68 

34.'3 

54^6 

88.9 

96 

37.8 

55.4- 

93.2 

105 

38.5 

55.6 

94.1 

142 

41.5 

55.8 

97.3 

(fitard,  A.  ch.  1894,  (7)  3.  286.) 

Solubility  of  mixed  crystals  of  KNO3  and 
AgNO3  in  H2O  at  25°. 


G.  per  1. 


AgNOs      KNOs 


45.9 
110.7 
X76.8 
259.6 
365.6 
507.9 
745.9 


321.8 
322.6 
333.7 
364.0 
456.4 
387.2 
398.6 


Mg.  mols.  per  1. 


AgNOs     KNOs 


270 
6513 
1040 
1258 
2151 
2988 
4388 


3180 
3184 
3298 
3597 
4511 
3816 
3960 


Mol.% 

AgNOs 

in  solu  - 

tion 


7.83 

16.96 
23.97 
29.81 
32.28 
43.85 
57.70 


Mol.% 
AgNOs 
in  solid 
phase 


0.2896 

0.6006 

0.9040 

1.054 

1.604 

2.439 

8.294 


(Groschuff,  Z.  anorg.  1904,  40.  10.) 


(Herz,  Z.  Kryst.  Min.  1897,  28.  405.) 


582 


NITRATE,  POTASSIUM 


Solubility  of  KNO3-fAgNO3  at  30°. 

Solubility  of 

KNO3+NaNO3  in  H2O  at  10°. 

Composition  of  the 
solution 

.     Solid  phase 

In  1000  ccm.  H2O 

Solid  phase 

NaNOs 

KNOs 

%  KNOs 

%  AgNOs 

805.0 

848.3 

301.9 
208.9 

NaNO3 
NaNO8,  KN03 
KNO? 

0 
5.53 
11.22 
13.44 
17.38 
25.05 
25.00 
26.58  ' 
29.22 
30.45 
31.30 

73.0 
71.65 
69.01 
65.08 
57.85 
46.32 
46.45 
39.09 
23.59 
11.51 
0 

AgN03 

u 

AgN03+AgN03,  KN03 
AgNO3,  KNO3 

KNO3+AgNO3,  KNO3 

KNO3 
n 

u 
(I 

(Kremann  and  Zitek,  M.  1909,  30.  325.) 
Solubility  of  KNO3+NaNO3  in  H2O  at  24.2°. 

In  1000  ccm.  H2O 

Solid  phase 

NaNOs 

KNOs 

913.58 
910.60 
1019.65 
1018.40 
931.30 
346.70 

123.60 
435.85 
437.70 
422.00 
390.00 
377.35 

NaNO3 

u 

NaN03,  KN03 
« 

KNO? 

u 

(Schreinemakers,  Z.  phys.  Ch.  1909,  65.  576.) 

KNO3+NaNO3. 
100  pts.  H2O  dissolve  34.53  pts.  KNO3  and 
91.16  pts.  NaNOg  at  15.6°,  and  solution  has 
sp.  gr.  =  1.478.    (Page  and  Keightley.) 
100  pts.  KNO3+NaNO3+Aq  sat.  at  14° 
contain  52.17  pts.  of  the  two  salts;  sat.  at  13° 
contain  53.15  pts.  of  the  two  salts,    (v.  Hauer.) 
100  pts.  H2O  dissolve  at  18.75°  29.45  pts. 
KNO3  and  89.53  pts.  NaNO3,  if  sat.  KNO3  + 
Aq  is  treated  with  NaNO3,  and  35.79  pts. 
KNO3  and  88.00  pts.  NaNO3  by  the  opposite 
process.    134.38  pts.  of  the  two  salts  are  dis- 
solved if  a  mixture  of  the  salts  is  treated  with 
H2O  at  18.75°.    (Karsten.) 
100  pts.  H2O  dissolve  39.34  pts.  KNO3  and 
94.60  pts.  NaNO3,  or  133.94  pts.  of  the  two 
salts  at  20°.    (Nicol,  Phil.  Mag.  (5)  13.  385.) 

(Kremann  and  Zitek.) 
Solubility  of  KNO3+NaNO3  in  H2O  at  25°. 

%  KN03 

%  NaNOs 

Solid  phase 

38.70 
41.60 
46.35 
39.08 
20.98 

39.62 
66.31 
100.10 
98.99 
94.44 

KN03 

u 

KNOs+NaNOs 

NaN03 

u 

(Uyeda,  Mem.  Col.  Sc.  Kioto,  1910,  2.  245.) 
Solubility  in  NaN03+Aq  at  20°,  30°,  40' 

Solubility  of  mixtures  of  KNO3  and  NaNO3. 


% 

NaNOs  in 
mixture 
before 
solution 

Total  amt. 
mixed 
salts  dis- 
solved in 
100  pts. 
H2O  at  20 

Pts. 
NaNOs 
dis 
solved 

Pts. 
KNOs 
dis 
solved 

NaNOs  in 
mixture 
after  solu- 
tion and 
evap.  to 
dryness 

100 

86.8 

86.8 

0 

100 

90 

109.6 

96.4 

13.2 

88 

80 

136.5 

98.0 

38.5 

71.8 

70 

136.3 

... 

60 

137.6 

9o!o 

47^6 

65^4 

50 

106.1 

66.0 

40.1 

62.2 

45.7* 

88.0 

53.3 

34.7 

60.6 

40 

81.1 

45.6 

35.6 

56.2 

30 

73.5 

20 

54.1 

26!  8 

33'3 

38.  5 

10 

40.9 

9.4 

31.5 

22.9. 

0 

33.6 

0 

33.6 

0 

*  NaNOs  +KNO3. 

(Carnelley   and   Thomson,   Chem.    Soc.   63. 

782.) 

and  91°.  Data,  given  in  the  original, 
that  each  salt  increases  the  solubility  of  th( 
other.  (Leather,  Mem.  Dept.  Agric.  India 
1914,  3.  177;  Chem.  Soc.  1915,  108.  (2),  13.) 
100  pts.  H2O  dissolve  28.92  pts.  KN03 
53.68  pts.  NaNO3,  and  26.44  pts.  NaCl  a 
15.6°,  and  solution  has  sp.  gr.  =  1.44.  (Pagi 
and  Keightley,  Chem.  Soc.  (2)  10.  566.) 

Solubility  of  KNO3+NaNO3+NaCl  in  H2( 
at  25°. 


KNOs 

ty 
NaNOs 

N&l 

Solid  phase 

38.44 
38.57 
42.55 
17.77 

28.08 
44.72 

22.87 
44.40 
63.26 
61.12 
62.92 
82.82 

32.58 
27.67 
23.59 
23.94 
23.70 
9.56 

NaCl+KNOs 
NaNOg,  KN03+NaC 

(Uyeda,  Mem.  Col.  Sc.  Kioto,  1910,  2.  245 

KN03+Sr(N03)2. 

1 1.  H2O  sat.  with  both  salts  at  25°  contau 
552  g.  KNO3+1074  g.  Sr(NO3)2.  (Le  Blar 
and  Noyes,  Z.  phys.  Ch.  1890,  6.  386.) 


NITRATE,  POTASSIUM 


583 


Solubility  of  KNO3+Sr(NO3)2  at  t°.  KNO3+KC1. 


KNOs 


% 
Sr(NOs 


Solid  phase 


100  pts.  H2O  dissolve  pts.  of  the  two  salts: 


20 


22.90 
21.70 
21.01 
19.60 
19.49 
19.69 
17.56 
12.65 
10 


5.49 
9.17 
17.10 
31.24 
34.91 
39.56 
40.37 
41.12 
40.70 


KNO3 


KNO3+Sr(NO3)2,  4H20 
Sr(NO3)2,  4H2O 


KNO3 
KC1 


At  12.9° 


18.8 
28.5 


At  15.3° 


18.9 
29.8 


40 


30.26 
26.90 
22.50 
11.19 
0 


23.70 
38.52 
40.22 
44.19 

47.7 


KNO3 

KNO3+Sr(NO3)2,  4H20 
Sr(NO3)2,  4H2O 


(Findlay,  Morgan  and  Morris,  Chem.  Soc. 
1914,  106.  779.) 

KNO3+TINQ3. 

100  g.  H2O  dissolve  43.5  g.  T1NO3+ 104.2  g 
KNO3  at  58°.  (Rabe,  Z.  anorg.  1902,  31. 
156.) 

Solubility  of  mixed  crystals  of  KNO3+T1NO3 
in  H2O  at  25°. 


(Kopp.) 


100  pts.  H2O  dissolve  315.2  pts.  KC1  and 
19.1  pts.  KNO3  at  20.0°.  (Riidorff,  B.  6.  484.) 

100  pts.  H2O  dissolve  18.95  pts.  KNO3+ 
32.84  pts.  KC1,  or  51.79  pts.  of  the  mixed 
salts  at  20°.  (Nicol,  Phil.  Mag.  (5)  31.  385.) 


Solubility  of  KC1  with  addition  of  KNO3  at 
17.5°. 


Sp.  gr. 


G.  per  1. 


TINOs 


0.00 
2.37 
6.15 
17.64 
49.74 
63.60 
86.18 
123.8 
101.3 
116.1 


KNOs 


351.0 
329.0 
332.4 
333.7 
333.3 
321.0 
330.5 
428.3 
245.1 
0.0 


Sp.  gr. 


.1730 
.1980 
.2100 
2250 
2360 
2390 
2388 
2410 


2632 

1903 

1956 

2050 

2196 

2436 

1.2617 

1.2950 

1.2050 

1.0964 


100  ccm.  of  solution  contain  g. 


KC1 


29.39 
27.50 
27.34 
26.53 
25.98 
25.96 
25.95 
26.24 


H2O 


87.85 
85.68 
84.76 
83.58 
82.84 
82.65 
82.43 
82.63 


KNOa 


0 

6.58 
8.83 
12.48 
14.83 
15.22 
15.49 
15.33 


KNO3  separated  out  in  last  four  solutions. 


Solubility  of  KNO3  with  addition  of  KC1  at 
20.5°. 


Sp.  gr. 


(Herz,  Z.  Kryst,  Min.  1897,  28.  405.) 
KN04+KBr. 

Solubility  in  KBr+Aq. 


1  litre  of  the  solution  contains 


at  14.5° 

at  25.2° 

Mol.  KBr 

Mol.  KNOs 

Mol.  KBr 

Mol.  KNOs 

0.0 

2.228 

0.0 

3.217 

0.356 

2.026 

0.38 

3.026 

0.784 

1.835 

0.93 

2.689 

1.092 

1.730 

1.37 

2.492 

1.577 

1.589 

2.08 

2.216 

2.5.42 

1.406 

2.87 

1.958 

3.536 

1.308 

3.55 

1.807 

1625 
1700 
1765 
1895 
1983 
2150 
2265 


1.2400 


100  ccm.  of  solution  contain  g. 


KN03 


27.68 
24.39 
22.44 
20.23 
18.96 
17.67 
17.11 
16.79 


H20 


88.51 
87.89 
87.47 
86.48 
85.69 
84.23 
83.40 
82.24 


KCl 


0 

4.72 
7.74 
12.23 
15.15 
19.61 
22.17 
24.96 


(Bodlander,  Z.  phys.  Ch.  7.  359.) 


(Touren,  C.  R.  1900,  130.  910.) 


584 


NITRATE,  POTASSIUM 


Solubility  in  KCl+Aq  at  t°. 

Solubility  of  KC1  in  KNO3+Aq. 

t° 

Sat.  solution  contains 

t 

Concentra- 
tion of 
KNOs 
%  mol.  per 

G.  salt 
dissolved  in 
1  1.  H20 

Molecular 
solubility 

%  KNOs 

%KC1 

%  total  salt 

—11.4 
—11 
—10 
—4 
+2.5 
4.5 
4.5 
8.5 
10.5 
13.5 
14 
17 
23 
27 
29 
34 
36 
37.5 
39 
42.5 
48 
50 
52 
53 
56 
61 
62 
71 
81 
85 
90 
96 
97 
104 
105 
120 
120 

4.0 
3.9 

3.8 

7^3 
7.8 
7.9 
8.4 
8.9 
10.2 
9.7 
12.5 
14.9 
16.1 
18.9 
18.9 
19.2 
21.0 
21.8 
25.3 
28.3 

29^5 
34.5 
35.4 
40.5 
47.1 
48.2 
52.8 
54.1 
56.6 
59.9 

69^6 
69.1 

18.4 
18.1 
18.6 
19.7 
19.9 
20.7 
19.8 
20.9 
21.0 
21.8 
21.3 
22.6 
21.8 
21.3 
21.0 
21.2 
21.6 
21.6 
21.0 
20.9 
20.3 
20.8 
20.2 

19^5 
18.3 

15^4 
15.3 
13.3 
12.6 
12.4 
10.8 
10.9 
7.7 
7.6 

22.4 
22.0 
22.5 

26^2 
28.0 
27.6 
28.8 
29.4 
30.7 
31.5 
32.3 
34.3 
36.2 
37.1 
39.3 
40.5 
40.8 
42.0 
42.7 
45.6 
49.1 

48.7 
49.0 

52.8 

57.'8 
62.5 
63.5 
66.1 
68.7 
69.0 
70.7 

77  .'3 

76.7 

0° 
25° 

0 

1 

0 

X 

1 

283.55 

284.25 
283.60 
287.60 
364.15 
365.00 
361.65 
358.80 
355.20 

3.81 
3.81 
3.81 
3.86 
4.89 
4.90 
4.86 
4.81 
4.77 

(Armstrong  and  Eyre,  Proc.  R.  Soc.  (A)  1910, 
84.  127.) 

Solubility  in  KCl+Aq  at  20°,  30°,  40°  and 
91°.    Data,  given  in  the  original,  show  that 
each  salt  diminishes  the  solubility  in  H2O  of 
the  other.  (Leather,  Mem.  Dept.  Agric.  India, 
1914,  3.  177;  Chem.  Soc.  1915,  108.  (2)  13.) 
KN03+NaCl. 
NaCl  is  sol.  in  sat.  KNO3+Aq,  and  the 
mixed  solution  is  capable  of  dissolving  more 
KN03.     An  amount  of  H2O,  which,  when 
pure,  could  only  dissolve  100  pts.  KNO3,  can 
in  this  way  be  made  to  take  up  152.64  pts. 
(Longchamp,  A.  ch.  (2)  9.  8.) 
Sol.  in  sat.  NaCl+Aq. 

100  pts.  H2O  dissolve: 

1/ongchamp 

Riidorff 

Page  and 
Keightlev 
15.6° 
(4) 

4° 

(1) 

14°            18° 
(2)             (3) 

NaCl 
KN03 

35.96 
26.01 

38.5     38.9 
28.7     36.1 

39.57 
32.32 

71.89 

(fitard,  A.  ch.  1894,  (7)  3.  285.) 
Solubility  in  KCl+Aq. 

61.97 

67.2    75.0 

Karsten 
18.75° 

Mulder 
At  b.-pt. 

(8) 

(5) 

(6)             (7) 

1  litre  of  the  solution  contains  at 

NaCl 
KNO3 

36.53      38.25     39.19 
33.12      29.45     38.53 

37.9 
306.7 

14.5° 

at  25.2° 

Mol.  KC1 

Mol.  KNOs 

Mol.  KC1 

Mol.  KNOs 

69.65      67.70    77.72 

344.6 

0.0 
0.182 
0.424 
0.880 

1.778 
2.204 
2.635 
3.172 

2.228 
2.172 
2.057 
1.830 
1.576 
1.515 
1.423 
1.355 

0.0 
0.26 
0.66 
1.35 

2.08 
2.78 
3.04 

3.217 
3.086 
2.853 
2.510 
2.218 
2.015 
1.946 

1,  2,  3,  4,  and  8.    I 
5.  Sat.  NaCl+Aq  1 
6.  Sat.  KNO3+Aq 
7.  The   two   salts 
with  H2O. 
100  pts.  H2O  dissol 
pts.  KC1,  and  38.58 
solution    has    sp.     g 
Keightley.) 

>oth  salts  in 
seated  with 
treated  with 
simultaneou 

ve  31.44  pts. 
pts.  NaCl  at 

excess. 
KNO3. 
NaCl. 
sly   treated 

KNO3,  139 
15.6°,  and 
Page    and 

(Touren,  C.  R.  1900,  130.  909.) 

r.  =  1.33. 

NITRATE,  POTASSIUM 


585 


Solubility  in  NaCl+Aq  at  t°. 

without  pptn.,  but  K2SO4  is  afterwards  pptd. 

Sat.  solution  contains 

(Karsten.) 

t° 

%  KNOs 

%  NaCl 

%  total  salt 

—22 

1Q     F: 

7.3 

7  Q 

22.5 

OQ     £* 

29.8 
Qn  a 

100  pts.  ±i2u  dissolve: 

—15.5 

/  .  \) 

8.7 

22'  1 

O(J.  O 

31.8 

Mulder 

Karsten             Kopp             Mulder 

—  7 

10.1 

22.5 

32.6 

18.75° 

18.75°      '  20o            40<T      18.75° 

—6 

10.9 

23.0 

33.9 

.  CD 

(2)            (3)              (4)           (5) 

i 

1O     ~" 

OO     O 

O/2     f\ 

—  i 
+1 

12.9 

28  ]§ 

oo.O 
36.7 

KNO3    29.90 

29.42    26.9     59.35 

+  11 

16.6 

22.8 

39.4 

K2SO 

4.0        6.6      5.75     10.8  ' 

17 

1  Q     A 

A  "I      O 

J.  / 

18 

19.8 

22'0 

41  .0 

41.8 

18 
20.5 

99 

18.9 
20.4 

22.5 
22.3 

41.5 

42.7 

2.  H2O  sat.  with  KNO3  and  K2S04  simul- 
taneously, or  to  a  sat.  solution  of  one  salt  the 

fm 

22 
26 
27 

21.8 
20.7 

20^7 
22.3 

42.'5 
43.0 

A  C     A 

other  was  added. 
3  and  4.    H2O  sat.  with  both  salts  simul- 
taneously. 

30.5 

24  7 

20  7 

45.0 
45.4 

Mulder  doubts  the  results  of  3  and  4. 

32.5 

25.0 

20.'2 

45.2 

32.5 

25.9 

20.2 

46.1 

33 
35 

26.7 
27.9 

20.7 
20.2 

47  .4 
48.1 

Solubility 

in  K2SO4+Aq  at  t°. 

39 

29  8 

19  5 

49.3 

42.2 

31.1 

20.0 

51.1 

In  100  ccm.  of  the  solution 

50 

38.5 

16.5 

55.0 

t 

np.  gr.  of 

54 

39.4 

17.1 

56.5 

G.  KNOa             G.  K2SO4           ~iuw«« 

58.5 
70 

40.9 
49.7 

15.3 
Mn 

56.2 

15           216.5               50.7              1.165 

76 

53^9 

.  \J 

13.6 

67!5 

25            308.5               47.66            1.210 

79 

54.8 

12.9 

67.7 

84 
90 

57.4 
61.4 

12.6 
10.4 

70.0 

71.8 

(Euler,  Z.  phys.  Ch.  1914,  40.  313.) 

96 

64.7 

9.5 

74.2 

105 

70.0 

9.0 

79.0 

106 

69.9 

9.3 

79.2 

Slowly  sol.  in 

sat.  Na?SO4  at  first  without 

107 

71.3 

8.4 

79.7 

pptn.,  but  afterwards  K2SO4  or  NaS04  sep- 

115 

72.2 

9.0 

81.2 

arates  out. 

122 

73.8 

8.0 

81.8' 

Sol.  in  sat.  ZnSO4+Aq  with  pptn.  of  double 

127 

73.6 

7.9 

81.5 

salt.    (Karsten.) 

127 

72.9 

8.8 

81.7 

Sol.  in  sat.  KClO3-f  Aq,  from  which  solu- 

127 

73.0 

7.6 

80.6 

tion  it  is  not  pptd.  by  salts  which  would  ppt. 

128 

74.2 

7.9 

82.1 

it  from  aqueous 

solution.     (Karsten.) 

132 

75.7 

7.6 

83.3 

Hydrazine  dissolves  21.7   pts.    KNO3   at 

145 

77.7 

7.6 

85.3 

12.5-13°.    (de  Bruyn,  R.  t.  c.  1899,  18.  297.) 

170 

80.7 

5.8 

86.5 

Neither  dissolved  nor  attacked  by  liquid 

171 

79.1 

5.9 

85.0 

NO2.    (Frankland,  Chem.  Soc.  1901,  79.  1361. 

Very  sol.  in  liquid  NH3.     (Franklin,  Am. 
Ch.  J.  1898,  20.  829.) 

(Etard,  A.  ch.  1894,  (7)  3.  283.) 

Insol.  in  absolute  alcohol;  in  dilute  alcohol 

100  g.  H2O  dissolve  41.14  g.  KNO3  and 
38.25  g.  NaCl  at  25°:  168.8  g.  KNO3  and 

on  o  i     _      XT_/~*«I        j     O/-YO           tc*       i        T         i              y--ii 

it  dissolves  proportional  to  the  amount  of  H2O 
present,  but  always  less  is  dissolved  than  the 
H2O  would  dissolve  by  itself.    (Gerardin.) 

(Soch,  J.  phys.  Ch. 
1898,  2.  46.) 

See  also  under  NaCl. 

Sol.  in  sat.  CuSO4-f-Aq,  forming  a  double 
salt,  which  soon  separates  out. 

Very  slowly  and  slightly  sol.  in  MgSO4  + 
Aq  with  pptn.  of  MgSO4.  (Karsten.) 

KNO3+K2SO4. 

Sat.  KNOe+Aq  dissolves  some  K2SO4,  and 
.sat.  K2SO4+Aq  slowly  dissolves  some  KNO3 


100  pts.  alcohol  containing  %  by  weight  of 
alcohol  dissolve  pts.  KNO3  at  15°. 

10     20     30     40     50     60     80%  alcohol 
13.2    8.5    5.6    4.3    2.8    1.7    0.4  pts.  KNO3. 

(Schiff,  A.  118.  365.) 


586 


NITRATE,  POTASSIUM 


Solubility  in  100  pts.  al< 
of  alcohol;  S 

;ohol 

att°.    D  =  sp.gr. 
lubility. 

Solubility  in  alcohol. 

—  so 

Wt.  %  alcohol 

G.  KNOs  per  100  g.  alcohol 

D  =0.9904 

D  =0.9848 

D  =0.9793 

D  =0.9726 

at  30° 

at  40° 

t° 

12 
21 
33 
43 
53 
61 
62 

s 

18.1 
25.0 
40.4 
58.6 
79.1 
94.5 
95.7 

t° 

s 

t° 

s 

t° 

S 

0 
8.25 
17.0 
25.7 
35.0 
44.9 
54.3 
65.0 
75.6 
88.0 

45.6 
32.3 
22.4 
15.1 
11.4(34.5°) 
7.0  ' 
4.5 
2.7 
1.3 
0.4 

64.5 
47.1 
33.3 
24.1 
16.7 
11.6(44°) 
7.2  (55°) 
4.4 
2.0(76.3°) 
0.6(88.5°) 

12 
21 
36 
41 
56 

14.6 
21.7 
37.8 
45.0 
72.9 

10 
10 
13 
18 
20 
31 
34 
40 
41 
50 
53 
61 
62 

10.20 
10.19 
11.74 
14.52 
16.35 
25.81 
28.63 
36.66 
37.20 
50.14 
56.01 
72.24 
73.36 

14 
25 
34 
•44 
47 
60 

8.8 
13.6 
20.3 
31.3 
34.2 
52.3 

(Bathrick,  J.  phys.  Ch.  1896,  1.  160.) 

Solubility  of  KNO3  in  ethyl  alcohol  +Aq  at 
30°. 

D  =0:9573 

D  =0.9390 

D  =0.8429 

D  —0.8967 

%  by  wt.  H2O      %  by  wt.  alcohol 

%  by  wt.  KNOs 

t° 

14 
25 
33 

44 
57 
65 

s 

5.4 
9.0 
13.2 
19.1 
29.1 
36.2 

t° 

16 
24 
40 
51 
60 
64 

S 

t° 

s 

t° 

S 

0.29 
0.39 
0.62 
0.78 
1.10 

68.7                    0 
69.2                   10.1 
67.3                   17.0 
64.1                  23.8 
58.8                  32.2 
50.8                  43.1 
39.8                  56.9 
33.9                  63.8 
22.3                  76.8 
7.5                  92.3 

31.3 
20.7 
15.7 
12.1 
9.0 
6.1 
3.3 
2.3 
0.88 
0.15 

4.13 
6.00 
10.94 
16.51 
21.54 
24.22 

12 
33 
47 
57 

1.61 
3.62 

5.77 
6.97 

15 
22 
40 
54 
60 

(Gerardin,  A.  ch.  (4)  5.  151.) 
Solubility  of  KNO3  in  alcohol  at  18°. 

(Schreinemakers,  Z.  phys.  Ch.  1909,  65.  556.) 
Solubility  in  ethyl  alcohol  at  25°. 

Sp.  gr. 

100  ccm.  contain  g. 

Alcohol 

Water 

KNOs 

Concentration  of         Soiubility  in 
alcohol  in  g.mol.             l  L  H£ 

p6F  1.   JT.2V/ 

Mol. 

solubility 

.1475 
.1085 
.1010 
.0805 
.0655 
.0490 
.0375 
0.9935 
0.9585 
0.9456 
0.9050 
0.8722 
0.8375 

3^30 
5.24. 
8.69 
14.08 
16.27 
19.97 
28.11 
37.53 
42.98 
51.23 
61.65 
69.60 

89.63 
87.44 
86.26 
83.18 
77.93 
76.36 
72.93 
64.74 
54.21 
48.15 
27.32 
24.74 
13.95 

25.12 
20.11 
18.60 
16.18 
14.54 
12.27 
10.85 
6.50 
4.11 
3.37 
1.95 
0.83 
0.20 

0                    384.48 
V*                    368.30 
V2                   354.40 
1                   327.00 

3.80 
3.64 
3.50 
3.22 

(Armstrong  and  Eyre,  Proc.  R.  Soc.  1910, 
(A)  84.  127.) 

Solubility  of  KNO3  in  methyl  alcohol  +Aq  at 
30°. 

%  by  wt.  H2O 

%  by  wt.  alcohol 

%  by  wt.  KNOs 

(Bodlander,  Z.  phys.  Ch.  7.  316.) 

68.7 
68.9 
66.4 
61.0 
53.9 
39.2 
0.99 

0 
7.8 
17.3 

27.8 
38.4 
57.0 

98.58 

31.3 
23.3 
16.3 
11.2 

7.7 
3.8 
0.43 

(Schreinemakers,  Z,  phys.  Ch.  1909,  65.  556.) 

NITRATE,  POTASSIUM  URANYL 


587 


Solubility     of     KNO3+AgNO3     in     51.6% 
C2H5OH+Aq  at  30°. 

Solubility  in  H2O. 

Solution  temp. 

%  by  wt. 
KN03 

%  by  wt. 
HN03 

%£<f- 

% 

KNOs 

% 

AgNQ3 

Solid  phase 

mpt.  +22° 
20.5 
18.0 
12.0 
6.0 
0 

44.5 
44.1 
43.8 
43.0 
42.3 
41.6 

55.5 
55.0. 
54.5 
53.6 
52.7 
51.8 

0 
0.9 
1.7 
3.4 
5.0 
6.6 

4.8 
4.55 
4.11 
4.26 
2.62 
0 

0 
5.15 
16.47 
21.28 
36.94 
37 

KN03 
it 

n 

KNO3+AgNO3,  KNO3 
AgNO3,  KNO3+AgNO3 
AgN03 

(Groschuff.  Z.  anore.  1904.  40.  11.) 

(Schreinemakers,  Z.  phys.  Ch.  1909,  65.  556.) 

100  g.  40%  ethyl  alcohol  sat.  with  KNO3  + 
NaCl  at  25°  contain  13.74  g.  KNO3+15.78  g. 
NaCl.  (Soch,  J.  phys.  Ch.  1898,  2.  43.) 

Insol.  in  propyl  alcohol.  (Schlamp,  Z. 
phys.  Ch.  1894,  14.  277.) 

Almost  insol.  in  ether.    (Braconnot.) 

Very  si.  sol.  in  acetone.  (Krug  and 
M'Elroy.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899.  II, 
1014.) 

Solubility  in  acetone -fAq  at  40°. 


Wt.  %  acetone 

G.  KNOs  per  100  g.  solvent 

0 

64.5 

8.5 

51.3 

16.8 

38.9 

25.2 

22.8 

34.3 

24.7 

44.1 

17.0 

53.9 

11.9 

64.8 

7.2 

76.0 

3.0 

87.6 

0.7 

(Bathrick,  J.  phys.  Ch.  1896,  1.  160.) 

100  pts.  glycerine  (sp.  gr.  1.225)  dissolve  10 
pts.  KN03.  (Vogel,  N.  Rep.  Ph.  16.  557.) 

100  g.  trichlorethylene  dissolve  0.01  g. 
KNO3  at  15°.  (Wester  and  Bruins,  Pharm. 
Weekbl.  1914,  51.  1443.) 

Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.257.)  f 

Insol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1370.) 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

100  g.  H2O  sat.  with  sugar  and  KNO3  dis- 
solve 224.7  g.  sugar  +  41.9  g.  KNO3,  or  sat. 
solution  contains  61.36  g.  sugar  +  11.45  g. 
KNO3  at  31.25°.  (Kohler,  Z.  Ver.  Zuckerind. 
1897,  47.  447.) 

Potassium  hydrogen  nitrate,  KN03,  HNO3. 

Very  hygroscopic.  Decomp.  by  H2O. 
(Groschuff,  B.  1904,  37.  1489.) 

Potassium  cfthydrogen  nitrate,  KNO3, 2HNO3. 
Decomp.  by  H2O.     (Ditte,  A.  ch.  (5)  18. 
320.) 


Potassium  silver  nitrate,  KNO3,  AgNO3. 

Sol.  in  H2O.  (Russell  and  Maskelyne,  Roy. 
Soc.  Proc.  26.  357.) 

3KNO3,  AgNO3.  Sol.  in  HoO.  (Rose, 
Pogg.  106.  320.) 

Potassium  thallic  nitrate,  2KNO3,  T1(NO3)3+ 

H20. 

Decomp.  by  H2O.  (Meyer,  Z.  anorg.  1900, 
24.  361.) 

Potassium  thorium  nitrate,  4KNO3,  Th(NO3)4. 
Very  sol.  in  H2O  and  alcohol.  (Berzelius.) 
Hydroscopic;  very  unstable.  (Meyer,  Z. 

anorg.  1901,  27.  379.) 
Hydroscopic;     sol.    in    dil.     HNO3+Aq. 

(Meyer,  Z.  anorg.  1901,  27.  378.) 

Potassium  thorium  hydrogen  nitrate,  3KNO3, 
Th(NO3)4,  3HNO3. 

Decomp.  in  the  air.  (Meyer,  B.  1900,  33. 
2140.) 

+4H2O.  Sol.  in  HNO3  of  1.2  sp.  gr. 
Effloresces  in  the  air.  f Meyer,  Z.  anorg. 
1901,  27.  380.) 

Potassium  uranyl  nitrate,  K(UO2)(NO3)3. 

Decomp.  by  H2O.  Sol.  in  cone.  HNO3. 
(Meyer,  B.  1903,  36.  4057.) 

Solubility  in  H2O  at  t°. 


t° 

In  100  pts. 
of  the  solution 

Solid  phase 

Pts.  by 

wt.U02 

Pts.  by 
wt.  K 

Pts.  by 
wt.  NOs 

0.5 

13.0 
25.0  a) 
b) 
45.0 
59.0 
80.6  a) 
b) 

31.98 

33.40 
37.08 
37.06 
42.18 
41.65 
43.72 
43.70 

1.72 

2.74 
4.05 
3.98 
5.16 
6.03 
6.42 
6.34 

23.49 
23.46 

Double  salt  + 
KN03 

Double  salt 

Potassium  uranyl  nitrate  is  decomp.  by 
H2O  at  temp,  below  60°;  above  60°  it  is 
sol.  in  H2O  without  decomp. 
(Rimbach,  B.  1904,  37.  473.) 

588 


NITRATE  BARIUM  SULPHATE,  POTASSIUM 


Potassium  nitrate  barium  sulphate,  KNO3, 
2BaSO4. 
Easily    decomp.      Sol.    in    cone.    H2SO4. 
(Silberberger,  M.  1904,  25.  251.) 

Potassium  nitrate  phosphomolybdate. 
See  Phosphomolybdate  nitrate,  potassium. 

Potassium  nitrate  sulphate,  KN03,  KHSO4. 
Decomp.  by  H2O  and  alcohol.   (Jacquelain.) 

Potassium  nitrate  sulphotungstate,  2KNO3, 
K2WS4  (?). 
Very  sol.  in  hot  or  cold  H20.     Insol.  in 
alcohol.    (Berzelius.) 

Solubility  in  H2O  at  t°. 

t° 

G.  PbNOs 
per  100  g. 

t° 

G.  RbNOs 
per  100  g. 

H20 

Solu- 
tion 

H2O 

Solu- 
tion 

0 
10 
20 
30 
40 
50 

19.5 

33.0 
53.3 
81.3 
116.7 
155.6 

16.3 
24.8 
34.6 
44.8 
53.9 
60.9 

60 
70 
80 
90 
100 
118.3 

200 
251- 
309 
375 
452 
617 

66.7 
71.5 
75.6 
78.9 
81.9 
86.1 

(Berkeley,  Trans.  Roy.  Soc.  1904,  203.  A. 
207.) 

Potassium  nitrate  tungstate  (?). 

100  pts.  boiling  H20  dissolve  5  pts.  salt. 
(Storer's  Diet.,  p.  393.) 

Potassium  nitrate  zinc  iodide. 

Permanent.  Easily  sol.  in  H2O.  Insol.  in 
alcohol.  (Anthon.) 

Praseodymium  nitrate,  Pr(NO3)3+6H2O. 

Sol.  in  H2O.  (von  Schule,  Z.  anorg.  1898, 
18.  355.) 

Praseodymium  rubidium  nitrate, 

[Pr(NO3)5]Rb2+4H2O. 
Hydroscopic.    (Jantsch,  Z.  anorg.  1911,  69. 
230.) 

Praseodymium    sodium    nitrate,    Pr(NO3)3, 

2NaN03+H20. 

Sol.  in  H2O.  (von  Schule,  Z.  anorg.  1898, 
18.  356.) 

Praseodymium     zinc     nitrate,     2Pr(NO3)3, 

3Zn(NO3)2+24H2O. 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  14.69  g.  hydrous  salt  at  16°. 
(Jantsch,  Z.  anorg.  1912,  76.  321.) 

Radium  nitrate. 

Has  apparently  the  same  solubility  in  H2O 
as  the  corresponding  Ba  comp.  (Curie,  Dis- 
sert. 1903.) 

Rhodium  nitrate,  Rh(NO3)3+2H2O  (?). 

Deliquescent.  Sol.  in  H2O.  Insol.  in 
alcohol.  (Glaus.) 

Rhodium  uranyl   nitrate, 

2(UO3)(NO3)2Rh2(NO3)6+10H2O. 
Sol.  in  H2O  and  acids;  insol.  in  aq.  alkalies 
(Lancien,  C.  C.  1912,  I.  208.) 

Rubidium  nitrate,  RbNO3. 

100  pts.  H2O  dissolve  20.1  pts.  at  0°;  43.5 
pts.  at  10°.  (Bunsen.) 


100  g.  H2O  dissolve  66.855  g.  RbNO3  at 
25°.  (Haigh,  J.  Am.  Chem.  Soc.  1912,  34. 
1148.) 

Sp.  gr.  20°/4°  of  a  normal  solution  of  RbNO3 

1.100835.;  of  a  0.5  normal  solution  =  1.04989. 
(Haigh,  J.  Am.  Chem.  Soc.  1912,  34.  1151.) 

Sp.  gr;  of  RbNO3 +Aq. 


r.-equiv.  RbNO3  per  1. 

at  18°  = 
Sp.  gr.  at  6°/6° 
Sp.  gr.  at  18°/18° 
Sp.  gr.  at  30°/30° 


0.5035     1.008 
1.05342  1.10566 
1.05226  1.10361 
1.05156  1.10222 


G.-equiv.  RbNO3  per  1. 

at  18°=  2.000      2.685 

Sp.  gr.  at  6°/6°  1.20655 

Sp.  gr.  at  18°/18°  1.20302  1.27066 

Sp.  gr.  at  30/30°  1.20036  1.26717 

(Clausen,  W.  Ann.  1914,  (4)  44.  1069.) 

Easily  sol.  in  HNO3.  (Schultz,  Zeit.  Ch. 
(2)  5.  531.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899,  II. 
1014;  Naumann,  B.  1904,  37.  4328.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Rubidium  hydrogen  nitrate,  RbNO3,  HNO3. 
Fairly  stable  in  air.     (Wells,  Am.  Ch.  J. 
1901,  26.  273.) 

Rubidium  ^hydrogen  nitrate,  RbNO3, 
2HNO3. 

Decomp.  rapidly  in  air.  (Wells,  Am.  Ch.  J. 
1901,  26.  273.) 

2RbNO3,  5HNO3.  Decomp.  by  H2O. 
Known  only  in  solution  in  HNO3-fAq. 
(Ditte,  A.  ch.  (5)  18.  320.) 

Rubidium  silver  nitrate,  RbNO3,  AgN03. 

Sol.  in  H2O.  (Russell  and  Maskelyne,  Roy. 
Soc.  Proc.  26.  357.) 

Rubidium  thorium  nitrate,  Rb2Th(NO3)6. 

SI.  sol.  in  HNO3;  decomp.  by  H2O.  (Meyer, 
Z.  anorg.  1901,  27.  384.) 


NITRATE,  SILVER 


589 


Rubidium  uranyl  nitrate,  Rb(UO2)(NO3)3. 
Decomp.  by  H2O.     Sol.  in  cone.  HNO3. 
(Meyer,  B.  1903,  36.  4057.) 

Solubility  of  H2O  at  t°. 

Solubility  in  H2O  at  t°. 
Sat.  AgNO3+Aq  contains  %  AgNO3  at  t°. 

t° 

%  AgNOs 

t° 

%  AgNOa 

—7 
—7 
—5 
—1 
—1 
+5 
10 
15.5 
20 
26 
29 
31 

46.2 
46.0 
47.6 
52.4 
51.9 
56.3 
61.2 
66.1 
67.8 
71.1 
73.0 
73.8 

36.5 
40.5 
45 
48 
73 
122 
134 
135 
135 
148 
160 
182 

75.7 

76.8 
77.1 
78.5 
84.0 
88.7 
92.1 
92.8 
92.7 
93.3 
95.2 
96.9 

t° 

25 

80 

In  100  pts.  of  the  solution 

Solid  phase 

Pts.  by 
wt.  UO2 

Pts. 
bv  wt. 
NOs 

Pts. 

Pts. 
by  wt. 
total 
salt 

a)  35.42 

b)  35.40 
a)  34.64 
b)  34  .  68 

19.72 
19.76 

4.63 

4.67 
11.01 
11.01 

59.57 

59.64 
69.46 
69.52 

Double  salt  + 
RbNO3 

Double  salt 

Rubidium  uranyl  nitrate  is  decomp.  by 
H2O  at  low  temp.;  at  80°  it  is  sol.  in  H2O 
without  decomp. 

(Rimbach,  B.  1904,  37.  476.) 


Samarium  nitrate,  Sm(NO3)3+6H2O. 

Easily  sol.  in  H29.    (Cleve,  C.  N.  48.  74.) 
Very    hydroscopic.      (Demarc.ay,    C.    R. 

1900,  130.  1187.) 


Samarium  zinc  nitrate,  2Sm(NO3)3, 

3Zn(NO3)2+24H2O. 

1  1.  sat.  solution  in  HNO3+Aq  (sp.  gr. 
1.325)  contains  36.47  g.  hydrous  salt  at  16°. 
(Jantsch,  Z.  anorg.  1912,  76.  321.) 


Scandium  nitrate,  basic. 

Sol.  in  H2O.    (Nilson,  B.  13.  1444.) 
ScOH(NO3)2+H2O.     (Crookes,  Roy.  Soc. 

Proc.  1908,  80.  A.  518.) 
Sc2O(NO3)4.    (Crookes.) 


Scandium  nitrate,  Sc(NO3)3. 

(Crookes,  Roy.  Soc.  Proc.  1908,  80.  A,  518.) 
+4H2O.    Very  sol.  in  H2O.    (Crookes.) 


Silver  nitrate,  AgNO3. 

100  pts.  H2O  at  11°  dissolve  127.7  pts. 
(Schnauss,  Arch.  Pharm.  (2)  82.  260.) 

100  pts.  H2O  dissolve  at: 

0°        19.5°     54°     85°     110° 
121.9      227.3      500    714     1111  pts.  AgNO3. 

(Kremers,  Pogg.  92.  497.) 


100  pts.  H2O  dissolve  1622.5  pts.  at  125°, 
and  1941.4  pts.  at  133°.  (Tilden  and  Shen- 
stone,  Phil.  Trans.  1884.  23.) 

Sat.  solution  boils  at  125°.    (Kremers.) 


(Etard,  A.  ch.  1894,  (7)  2.  526.) 

100  g.  sat.  AgNO3+Aq  at  15.5°  contain 
65.5  g.  AgNO3.  (Greenish  and  Smith,  Pharm. 
Jour.  1903,  71.  881.) 

Solubility  of  AgNO3  in  H20  at  30°  =  10.31 
mol.-litre.  (Masson,  Chem.  Soc.  1911,  99. 
1136.) 

100  g.  AgNO3+Aq  sat.  at  30°  contain  73.0 
g.  AgN03.  (Schreinemakers  and  de  Baat, 
Arch.  Neer.  Sc.  1911,  (2)  15.  415.) 

100  g.  sat.  AgNO3+Aq  contain  53.5  g. 
AgNO3  at  0°;  66.7  g.  at  18°.  (Mylius,  Z. 
anorg.  1912,  74.  411.) 

Sp.  gr.  of  aqueous  solution,  according  to 
C.  K.  =  Chemiker  Kalender;  K.  M.=Kohl- 
rausch  by  Mendelejeff  (Z.  anal.  27.  284);  and 
K  =  Kohlrausch  (W.  Ann.  1879.  1),  contain- 
ing: 

C.K. 
K.  M. 
K. 


5 

10 

15 

20%  AgN03, 

1.041 

1.080 

1.125 

1.160 

1.0440 

1.0901 

1.1969 

1.0422 

1.0893 

1.1404 

1.1958 

25 

30 

35 

40%  AgN03, 

1.206 

1.251 

C.  M 1.4791 

K.          1.2555    1.3213    1.3945    1.4773 

45       50%  AgNO3. 
K.         .1.5705    1.6745 

Sp.  gr.  of  AgNOs+Aq  at  25°. 


Concentration  of  AgNOa 

Sp.  gr. 

1-normal 

Vr-      " 
Vr-      " 
Vr-      " 

1.1386 
1.0692 
1.0348 
1.0173 

(Wagner,  Z.  phys.  Ch.  1890,  5.  40.) 

Sol.  in  500  pts.  HNO3;  30  pts.  2HNO3, 
3H2O  at  20°;  and  6  pts.  2HNO3,  3H2O  at  100°. 
(Schultz,  Zeit.  Ch.  1869.  531.) 

Insol.  in  cone.  HNO3.  (Warren,  C.  C. 
1897.  I,  438.) 


590 


NITRATE,  SILVER 


Solubility  of  AgNO3  in  HNO3+Aq  at  25°. 

•  Only  traces  are  sol.  in  absolute  alcohol  or 
ether.    100  pts.  of  a  mixture  of  1  vol.  alcohol 
(95  vol.  %)+!  vol.  pure  ether  dissolve  1.6 
pts.  AgNO3  at  15°;  100  pts.  of  2  vols.  alcohol 
+1    vol.    ether    dissolve    2.3    pts.    AgNO3. 
(Eder,  J.  pr.  1878,  (2)  17.  45.) 

Solubility  of  AgNO3  in   ethyl  alcohol  +Aq 
at  30°. 

G.  mol.  per  1. 

G.  AgNOs 
per  1. 

SP.  gr.  25° 

HNOs 

AgNOs 

0 
0.404 
0.962 
1.698 
2.834 
4.497 
5.992 
8.84 
12.53 

10.31 
9.36 
8.08 
6.54 
4.526 
2.590 
1.698 
0.843 
0.347 

1752 
1591 
1373 
1111 
769.1 
440.1 
288.6 
143.2 
58.90 

2.3921 
2.2754 
2.1243 
.9402 
.7052 
.4980 
.4195 
.3818 
.3976 

%  by  wt.  H2O 

%  by  wt.  alcohol 

%  by  wt.  AgNOs 

27.0 
27.71 
30.80 
32.10 
31.40 
28.95 
27.91 
20.92 
6.83 

2^8 
13.67 
20.13 
25.85 
37.26 
44.54 
64.42 
86.54 

73.0 
69.49 
55.53 
47.77 
42.75 
33.79 
27.55 
14.66 
6.63 

(Masson,  Chem.  Soc.  1911,  99.  1132.) 

AgNO3+NH4NO8.     Solubility  of  AgNO3 
in  NH4NO3+Aq.    See  under  NH4NO3. 
AgNO3  +KN03.      Solubility    of    AgNO3 
+KNO3  in  H20.    See  under  KNO3. 

AgN03+AgN02. 
Solubility  of  AgNO3+AgNO2  at  18°. 

(Schreinemakers,  Z.  phys.  Ch.  1909,  65.  571.) 

Solubility  of  AgNO3+KNO3  in   alcohol. 
See  under  KN03. 
Sol.  in  methyl,  ethyl,  and  isobutyl  alcohols, 
CC14,  CHC13,  acetone  and  pyridine.    (Wilcox, 
J.  phys.  Chem.  1910,  14.  587.) 
100  pts.  H2O  sat.  with  ether  dissolve  88.4 
pts.  AgNO3  at  15°.    (Eder,  I.  c.) 
Sol.  in  glycerine. 
Sol.  in  benzonitrile.     100  g.  benzonitrile 
dissolve  about  105  g.  AgNO3  at  18°.    (Nau- 
mann and  Schier,  B.  1914,  47.  1369.) 
1  pt.  acetonitrile  dissolves  about  1.5  pts. 
AgNO3.    (Scholl  and  Steinkopf,  B.  1906,  39. 
4398.) 

G.  per  1. 

G.  per    . 

AgNOs 

AgNOa 

AgNOs 

AgNO2 

0.000 
0.439 

0.878 
1.756 

3.184 
3.042 
2.926 
2.601 

3.512 
7.024 
14.048 

2.201 
1.799 
1.480 

(Naumann  and  Rucker,  B.  1905,  38.  2293.) 
See  also  under  AgNO2. 

Insol.  in  liquid  CO2.  (Biichner,  Z.  phys. 
Ch.  1906,  54.  674.) 

Very  sol.  in  liquid  NH3.  (Franklin,  Am. 
Ch.  J.  1898,  20.  829.) 

Sol.  in  4  pts.  boiling  alcohol. 

Sol.  in  10  pts.  alcohol.    (Dumas.) 

Sol.  in  11  pts.  alcohol  of  90%.    (Hager.) 

Solubility  in  100  pts.  alcohol  of  given  vol.  % 
att°. 


t° 

95% 

80% 

70% 

.60% 

15 
50 
75 

3.8 
7.3 
18.3 

10.3 
42!o 

22.1 

30.5 
58.1 
89.0 

t° 

50% 

40% 

30% 

20% 

io% 

15 
50 
75 

35.8 

56.4 
98.3 
160 

73.7 

107 
214 
340 

158 

(Eder,  J.  pr.  (2)  17.  44.) 

100  pts.  absolute  methyl  alcohol  dissolve 
3.72  pts.  at  19°;  100  pts.  absolute  ethyl  al- 
cohol dissolve  3.1  pts.  at  19°.  (de  Bruyn,  Z. 
phys.  Ch.  10.  783.) 


Easily  sol.  in  methyl,  ethyl,  and  amyl 
amine.  (Shinn,  J.  phys.  Chem.  1907, 11.  538.) 

Sol.  in  acetone.  (Krug  and  M'Elroy,  J. 
Anal.  Ch.  6.  184.) 

0.35  pts.  are  sol.  in  100  pts.  acetone  at  14°. 
0.35     "    "     "      "  100    "          "       "  59°. 
(Laszyznski,  B.  1894,  27.  2287.) 

Sol.  in  acetone  and  in  methylal.  (Eidmann, 
C.  C.  1899,  II.  1014.) 

1  g.  AgN03  is  sol.  in  227  g.  acetone  at  18°. 
Sp.  gr.  of  sat.  solution  18°/4°  =  0.798.  (Nau- 
mann, B.  1904,  37.  4339.) 

Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.  257.) 

Difficultly  sol.  in  methyl  acetate.  (Nau- 
mann, B.  1909,  42.  3790.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1904,  37.  3601.) 

Sol.  in  urethane.  (Castoro,  Z.  anorg.  1899, 
20.  61.) 

100  g.  C6H6  dissolve  0.022  g.  AgNO3  at  35°; 
0.044  g.  at  40.5°.  (Linebarger,  Am.  J.  Sci. 
1895,  49.  48.) 

Mol.  weight  determined  in  piperidine, 
pyridine  and  benzonitrile.  (Werner,  Z.  anorg. 
1897,  15.  pp.  17,  -23  and  32.) 


NITRATE,  SODIUM 


591 


Solubility  of  AgNO3  in  pyridine  at  t°. 

Silver  nitrate  antimonide,  AgNO3,  Ag3Sb. 

t° 

G.  AgNoa 
per  100  g. 

Solid  phase 

Decomp.  at  once  by  H2O.     (Poleck  and 
Thummel,  B.  16.  2435.) 

CsH5N 

Silver  nitrate  arsenide.  AgNO3  Ao'sAs. 

-48.5°* 

0 

C5H5N 

Decomp.  at  once  by  H2O.     (Poleck  and 

-50.5 

3 

" 

Thummel.) 

-53 

6 

" 

-59 

9 

M 

Silver  nitrate  bromide,  AgNO3,  AgBr. 

-65 
-51.25 

li'.l 

C5H6N+AgNO3,  6C5H6N 
AgNO3,  6C6H5N 

Decomp.  immediately  by  H2O  or  alcohol, 
with  separation  of  AgBr.    (Risse,  A.  111.  39.) 

—44 

11  7 

f 

-40 

12.2 

" 

Silver  nitrate  chloride,  AgNO3,  AgCl. 

-35 

12.6 

(t 

Quickly  decomp.  with  H2O;  more  slowly 

-30 

13.9 

" 

with  absolute  alcohol;  not  decomp.  by  ether- 

-25 

17.6 

M 

alcohol.    (Reichert,  J.  pr.  92.  237.) 

-24 
-22 
-10 

18.8 
20.03 

"      +AgNO3,  3C5H6N 
AgNO3,  3C6H6N 

Silver  nitrate  cyanide,  2AgNO3,  AgCN. 
Decomp.  by  H2O,  not  by  alcohol.     (Hell- 

0 

22.34 

it 

wig,  Z.  anorg.  1900,  25.  177.) 

+10 

27.21 

" 

Silver  nitrate  iodide,  AgNO3,  Agl. 

20 
30 
40 

A  e 

33.64 
40.86 
53.52 

ci 

a 

Cold  H2O  separates  Agl,  which  redissolves 
on  heating.     (Stiirenberg,  Arch.  Pharm.  (2) 
143.  12.)    Sol.  in  little  H2O  without  decomp.; 

to 
46 

A*l 

63!  06 

£?£»    ocr 

(C 

more  H2O  separates  Agl.     (Kremers,  J.  pr. 
71.  54.)     Insol.  in  absolute  alcohol.    Sol.  in 

47 
48 
48.5 
45 

66.35 
70.85 

69^85 

11 

"      +AgN03,2C5H6N 
AgN03,  2C5H5N 

cone.  AgN03+Aq. 
2AgNO3,  Agl.    Sol.  in  little  but  decomp.  by 
more  boiling  H2O.    (Risse,  A.  111.  39.) 

50 

72.25 

1 

Silver  nitrate  mercuric  oxide,  AgNO3,  2HgO. 

60 

78.60 

i 

Decomp.    bv   H2O.      Sol.   in   HNO3   and 

70 

89.10 

' 

H2SO4.     (Find,  Gazz.  ch.  it.  1910,  41.  (2) 

80 

121.21 

' 

548.) 

87 
80 

215.02 
228.5 

« 

Silver  nitrate  phosphide,  3AgNO3,  Ag3P. 

74 

230.6 

" 

(Warren,  C.  N.  56.  113.) 

74 
80 

235.4 
230  4 

" 

Silver  nitrate  silicide,  4AgNO3,  AgSi. 

87 

237  !l 

(t 

(Buchner,  Ch.  Ztg.  9.  484.) 

90 

241.9 

" 
" 

Silver  nitrate  silicate,  2AgNO3,  3Ag4SiO4. 

100 
110 

253.8 
271.4 

Sol.  in  dil.  HN03+Aq,  but  SiO2  separates 
out  after  heating.    (Rousseau  and  Tite,  C.  R. 

*  M.  pt. 

114.  294.) 

(Kahlenberg  and  Brewer,  J.  phys.  Ch.  1908, 

Silver  nitrate  sulphide,  AgNO3,  Ag2S. 

12.  283.) 

Decomp.  by  H2O.    (Poleck  and  Thummel, 

B.  16.  2435.) 

Silver  nitrate  acetylide,  AgNO3,  AgHC2. 

(Willgerodt,  B.  1895,  28.  2108.) 

AgNO3,  Ag2C2.  Ppt.  (Chavastelon,  C.  R. 
1897,  124.  1365.) 

2AgNO3,  Ag2C2.    (Chavastelon.) 

Silver  nitrate  ammonia,  AgNO3,  NH3. 

Partly  sol.  in  H2O;  rather  sol.  in  alcohol. 
SI.  sol.  in  ether.  (Reychler,  B.  16.  990.) 

Very  sol.  in  liquid  ammonia  below  — -10°. 
(Joannis,  C.  R.  1894,  118.  1151.) 

AgNO3,  2NH3.  Easily  sol.  in  H2O.  (Mit- 
scherlich.) 

1 1.  alcohol  dissolves  0.0383  g.  mols.  (Kuri- 
low,  C.  C.  1903.  II,  97.) 

AgNO3,  3NH3.  Completely  sol.  in  H2O. 
(Rose,  Pogg.  20.  153.) 


Silver  nitrate  sulphocyanide,  2AgN03, 

AgSCN. 

Decomp.  by  H2O,  not  by  alcohol.  (Hellwig, 
Z.  anorg.  1900,  25.  178.) 

Sodium  nitrate,  NaNO8. 

Deliquescent  in  moist  air.  Sol.  in  H2O  with 
absorption  of  heat.  75  pts.  NaNO3  mixed 
with  100  pts.  H2O  at  13.2°  lower  the  tempera- 
ture 18.5°.  (Riidorff,  B.  2.  68.) 


Sol.  in  1.58  pts.  H2O  at  —  6°. 
0.46 
2.89 
1.12 
0.79 
1.14 
1.136 
1.16 


(Marx.) 
(Osann.) 


+119°. 
2°. 
28°. 
47°. 

18.5°.       (Kopp.) 
18  75°.     (Karsten.) 
20°.    (Schiff,  A.  109.  326.) 
18.75°.     (Abl.) 


592 


NITRATE,  SODIUM 


100  pts.  H2O  at  t°  dissolve  pts.  NaNO3. 

Solubility  in  100  pts.  H2O  at  t°. 

t° 

Pts.  NaNOs 

t° 

Pts.  NaNOs 

t 

Pts.  NaNOs 

t° 

Pts.  NaNO3 

—6 

68.80 

50 

111.13 

0 

72  9 

60 

122 

0 

79.75 

60 

119.94 

1 

74.7 

61 

124 

10 

84.30 

70 

129.63 

2 

75.4 

62 

125 

16 

87.63 

80 

140.72 

3 

76.0 

63 

126 

20 

89.55 

90 

153.63 

4 

76.7 

64 

127 

30 

95.37 

100 

168.20 

5 

77  4 

65 

128 

40 

102.31 

120 

225.30 

6 

78.1 

66 

130 

(Poggiale,  A.  ch.  (3)  8.  469.) 

7 
8 

78.7 
79.4 

67 
68 

131 
132 

100  pts.  H2O  at  119°  dissolve  150  pts.  NaNOs.    (Grif- 

9 

80.1 

69 

133 

fiths.) 
NaNOs  +  Aq  sat.  at  18.75°  has  1.3769  sp.  gr.,  and  100 
pts.  H2O  have  dissolved  88.001  pts.  NaNOs.     (Kar- 

10 
11 

80.8 
81.4 

70 
71 

134 
136 

sten.) 

12 

82.0 

72 

137 

NaNOs  +Aq  sat.  in  cold  contains  33.3%    NaNOs. 
(Fourcroy.) 
NaNOs  +Aq   sat.    at    12.5°   contains   34%    NaNOs. 

13 
14 

82.7 
83.4 

73 

74 

138 
139 

(Hassenfratz.) 

15 

84.0 

75 

140 

100  pts.  H2O  at  15.5°  dissolve  33  pts.;  at  52°,  100  pts. 
NaNOs.     (Ure's  Diet.) 

16 
17 

84.7 
85.4 

76 

77 

142 
143 

100  pts.  H2O  dissolve  pts.  NaNO3  at  t°. 

18 

86.1 

78 

145 

QC     Q 

7Q 

-\  A  a 

t° 

Pts.  NaNOs 

t° 

Pts.  NaNOs 

20 

ou  .  o 

87.5 

i  \) 

80 

11O 

148 

0 

73.0 

60.65 

125.5 

21 
22 

88.3 
89.0 

81 
82 

149 
151 

13.9 

81.6 

99.9 

173.6 

23 

89  7 

83 

152 

44.65 

110.5 

119.7 

211.4 

24 

90.3 

84 

153 

(Nordenskjold,  Pogg.  136.  312.) 

25 

26 

91.0 
91.8 

85 
86 

155 
156 

100  pts.  H2O  dissolve  pts.  NaNO3  at  t°. 

27 

92.5 

87 

00 

158 

1  KQ 

t° 

Pts.  NaNOs 

t° 

Pts.  NaNOs 

29 

94^0 

oo 

89 

loy 
161 

0 

70.94 

70 

142.31 

30 
31 

94.9 
96.0 

90 
91 

162 
164 

10 

78.57 

80 

153.72 

32 

96 

92 

166 

20 

87.97 

90 

165.55 

33 

97 

93 

168 

30 

98.26 

100 

178.18 

34 

98 

94 

169 

40 

109.01 

110 

194.26 

35 

99 

95 

171 

50 

120.00 

119.4 

213.43 

36 

100 

96 

173 

60 

131.11 

37 

100 

97 

175 

(Maumen£,  C.  R.  58.  81.) 

38 
39 

101 
102 

98 
99 

177 
178 

100  pts.  NaNOs  4-  Aq  sat.  at  14°  contain 
43.88  pts.  NaNO3;  at  15°,  44.53  pts.  NaNO3. 
(v.  Plauer,  J.  pr.  98.  137.) 
100   pts.   H2O   dissolve   84.21-84.69   pts. 
NaNOs  at  15.6°,  and  sat.  solution  has  sp.  gr. 
1.337-1.378.     (Page  and  Keightley,  Chem. 
Soc.  (2)  10.  556.) 

40 
41 
42 
43 
44 
45 
46 
47 

102 
103 
104 
105 
106 
107 
108 
109 

100 
101 
102 
103 
104 
105 
106 
107 

180 
182 
184 
186 
188 
190 
192 
194 

100  pts.  H2O  dissolve  pts.  NaNO3  at  t°. 

48 

110 

108 

196 

t° 

Pts.  NaNOs 

t° 

Pts.  NaNOs 

49 
50 

111 
112 

109 
110 

198 
200 

0 
2 
4 
8 
10 
13 
15 

66.69 
70.97 
71.04 
75.65 
76.31 
79.00 
80.60 

18 
21 
26 
29 
36 
51 
68 

83.62 
85.73 
90.33 
92.93 
99.39 
113.63 
125.07 

51 
52 
53 
54 
55 
56 
57 
58 

113 
114 
115 
116 
117 
118 
119 
120 

111 
112 
113 
114 
115 
116 
117 
117.5 

202 
204 
207 
209 
211 
213 
215 
216.4 

Solubility  is  constant  from  0°  to  —15.7°, 

59 

211 

when  NaNO3  +7H2O  separates  out.     (Ditte, 

C.  R.  80.  1164.) 

(Mulder,  Scheik.  Verhandel.  1864.  83.) 

NITRATE,  SODIUM 


593 


v.i.Tj.ciuiiicjj.0/  ,    ^JL-L.-I:    j_/i»a.    j.^a.x^v/3    v-i-^ uiuciisi^juiu.^  ,    ^ 

pts.  NaNOs  (Legrand) ;  150  pts.  NaNOs  (Griffiths) 

Sat.  NaNO3 +Aq  contains  at: 
120°      130°      172°      180°      199° 
66.8      67.5      77.1       78.1       82.0%  NaNO3, 

220°      250°      255°      290°      313°  (mpt.). 
83.5      89.5      91.5      97.5       100%  NaNO3. 
(fitard,  A.  ch.  1894,  (7)  2.  527.) 

100  g.  sat.  NaNOs+Aq  contain  42.47  g. 
NaNO3  at  0°.  (Coppadoro,  Rass.  Min.  1911, 
XVII,  35.  123.) 

100  g.  sat.  NaNOs+Aq  contain  49.16  g. 
NaNO3  at  30°.  (Coppadoro,  Rass.  Min. 
1912,  37.  7.) 

100  g.  H2O  dissolve  92.14  g.  NaNO3  at  25°. 
(Haigh,  J.  Am.  Chem.  Soc.  1912,  34.  1148.) 

The  solubility  of  crystals  on  different  faces 
has  been  determined  by  Lebrun.  (Belg.  Acad. 
Bull.  1913.  953.) 

Sp.  gr.  of  NaNOs+Aq  at  19.5°. 


%  NaNOi 


12.057 
22.726 
31.987 


Sp.  gr. 


1.0844 
1 . 1667 
1.2450 


%  NaNOs 

39.860 
46.251 


Sp.  gr. 


1.3176 
1.3805 


(Kremers,  Pogg.  95.  120.) 
Sp.  gr.  of  NaNO3+Aq  at  20.2°. 


Sp.  gr.  of  NaNO3+Aq  at  18°. 


%  NaNOs 

Sp.  gr. 

%  NaNOs 

Sp.  gr. 

5 
10 

1.0327 
1.0681 

20 
30 

1.1435 
1.2278 

(Kohlrausch,  W.  Ann.  1879.  1.) 

Sp.  gr.  of  NaNOs+Aq  at  20°,   containing 
mols.  NaNO3  in  100  mols.  H2O. 


Mols.  NaNOs 

Sp.  gr. 

2 

5 

1.05980 
1  .  13813 

(Nicol,  Phil.  Mag.  (5)  16.  122.) 


The  saturated  solution  boils  at  1 17.5°.  (Mulder.) 

118.9°.  (Griffiths.) 

119°.  (Marx.) 

119.4°.  (Maumene.) 

119.7°  (Nordenskjold.) 

121°.  (Legrand.) 
122-123°.    (Kremers.) 

NaNOs+Aq  forms  a  crust  at  118°,  and 
contains  194  pts.  NaNO3  to  100  pts.  H2O; 
highest  temp,  observed,  120.5°.  (Gerlach,*Z. 
anal.  26.  427.) 


B.-pt.  of  NaNO3+Aq  containing  pts.  NaNOg 
to  100  pts.  H2O.  G=  according  to  Ger- 
lach  (Z.  anal.  26.  433);  L  =  according  to 
Legrand  (A.  ch.  (2)  59.  431). 


%  NaNOs 


Sp.  gr. 


%  NaNOs 


Sp.  gr. 


B.-pt. 


B.-pt. 


G 


1 

2 

3 

4 

5 

6 

7 

8 

9 

10 

11 

12 

13 

14 

15 

16 

17 

18 

19 

20 

21 

22 

23 

24 

25 


1.0065 

1.0131 

1.0197 

1.0264 

1.0332 

1.0399 

1.0468 

.0537 

.0606 

.0676 

.0746 

.0817 

.0889 

.0962 

.1035 

.1109 

.1184 

.1260 

.1338 

.1418 

.1498 

.1578 

.  1659 

1.1740 

1 . 1822 


26 
27 
28 
29 
30 
31 
32 
33 
34 
35 
36 
37 
38 
39 
40 
41 
42 
43 
44 
45 
46 
47 
48 
49 
50 


1 . 1904 
1 . 1987 
1.2070 
1.2154 
1.2239 
1.2325 
1.2412 
1.2500 
1.2589 
1.2679 
1.2770 
1.2863 
1.2958 


101° 
102 
103 
104 
105 
106 
107 
108 
109 
110 
111 


18.5 
28 
38 
48 
58 
68 

78.5 
89 
99.5 
110.5 


9.3 

18.7 
28.2 
37.9 
47.7 
57.6 
67.7 
77.9 
88.3 
98.8 
109.5 


112C 
113 
114 
115 
116 
117 
118 
119 
120 
121 


121. 

133 

144. 

156 

168. 

181 

194 

207. 

222 


120.3 
131.3 
142.4 
153.7 
165.2 
176.8 
188.6 
200.5 
212.6 
224.8 


3055 
3155 
3225 
3355 


1.3456 


1.3557 
1.3659 
1.3761 
1.3864 
1.3968 
1.4074 
1.4180 


50  pts.  NaNOs  mixed  with  100  pts.  snow  at 
— 1°  give  a  temp,  of  —17 . 5°.  (Riidorff,  Pogg. 
122.  337.) 


Sp.  gr.  of  NaN03+Aq  at  t°. 


G.  NaNOs  dis- 
solved in  100  g. 
H20 


(Schiff,   calculated  by  Gerlach,  Z.  anal.  8. 
280.) 


4.166 
11.111 
25.000 


G.  NaNOs  in 
100  g.  of  the 


4 

10 
20 


17.8° 

13.9° 

12° 


Sp.  gr. 


1.0276 
1.0704 
1.1441 


(de  Lannoy,  Z.  phys.  Ch.  1895,  18.  465.) 


594 


NITRATE,  SODIUM 


Sp.  gr.  of  NaNO3+Aq  at  2C 
per  cent  strength  of  sol 
density:    w=  volume    cc 

/pd          \ 
percc.(joo  =  w  j 

1.1°,  when  p  = 

Solubility  of  NaNO3  in  NH4OH+Aq  at  15°. 

nc.    in    grams 

G.  per  100  g.  H2Q 

Sp.  gr. 

NH3 

NaNOs 

13.87 

17.28 
20.38 

75.03 
73.99 
73.18 

1.253 
1.233 
1.212 

P 

d 

w 

42.05 
35.65 
31.72 
23.24 
17.370 
11.915 
9.665 
7.039 
4.241 
1.589 

1.3380 
1.2765 
1.2407 
1.1696 
1.1228 
1.0819 
1.0656 
1.0468 
1.0273 
1.0096 

0.56267 
0.45510 
0.39365 
0.27180 
0.19505 
0.12888 
0.10300 
0.07369 
0.04357 
0.01604 

(Fedotieff  and  Koltunoff,  Z.  anorg.  1914,  86. 
251.) 

NaNO3+Na2CO3.    (See  Na2CO3.) 
Sol.  in  sat.  NH4Cl+Aq. 
Very  rapidly  sol.  in  sat.  BaCl2+Aq  with 
pptn.  of  Ba(NO3)2. 
Sol.  in  sat.  KCl+Aq,  with  formation  of 
KN03. 
Sol.  in  sat.  NH4NO3+Aq.    (See  NH4NO3.) 
Sol.  in  sat.  Ba(NO3)2+Aq,   with  partial 
pptn.  of  Ba(NO3)2.    (See  Ba(NO3)2.) 
Sol.  in  sat.  Pb(NO3)2+Aq,  with  subsequent 
pptn.  of  Pb(NO3)2.    (See  Pb(NO3)2.) 
NaN03+KN03. 
Sol.  in  sat  KNO3+Aq;  solution  thus  made 
at  18°  contains  54.33%  mixed  salt,  or  100  pts. 
H2O   dissolve   118.98  pts.   mixed  salt,   viz. 
89.53   pts.   NaN03   and  29.45   pts.   KNO3. 
(See  KNO3.) 
NaNO3+Sr(NO3)2. 
If  Sr(NO3)2+Aq  sat.  at  14.5°  is  sat.  with 
NaNO3,  100  pts.  H2O  dissolve: 

(Barnes,  J.  phys.  Chem.  1898,  2.  545.) 

Sp.  gr.  20°/4°  of  a  normal  solution  of  NaNO3 
=  1.05386;  of  a  0.5  normal  solution  =  1.02646. 
(Haigh,  J.  Am.  Chem.  Soc.  1912,  34.  1151.) 

Sp.  gr.  of  sat.  NaNOs+Aq  at  t°. 

t° 

G.  NaNOs  sol. 
in  100  g.  H20 

Sp.  gr. 

—10 
0 
10 
20 

68.0 

43.0 
80.5 
88.0 

1.342 
1.358 
1.377 
1.387 

Sol.  in  66  pts.  HNO3;  in  32  pts.  2HNO3, 
3H2O  at  32°;  in  4  pts.  2HNO3,  3H2O  at  123°. 
(Schultz,  Zeit.  Ch.  (2)  6.  531.) 

Solubility  in  HNO3+Aq  at  0°. 


NaNO3 
Sr(N03)2  .     . 

83.7 

66.4 
51.0 

62'!  6 

117.4 

(Mulder.) 


NaNO,+NaNO2.  See  under  NaNO2. 
NaNO3+NaCl. 

100  pts.  H2O  dissolve  24.91  pts.  NaCl-f 
54.55  pts.  NaNO3  =  79.46  pts.  of  the  two  salts 


G.  per  100  cc.  of  solution 

at  20°. 

(Nicol,  Phil.  Mag. 

(5)  31. 

386.) 

Sp   gr 

NaNOs 

HNOs 

100  pts.  H2O 

dissolve  at  18.75°: 

56.5 

0.00 

341 

54.2 

e-i     40 

1.67 

3CQ 

.338 

001 

1 

•      2 

3 

4 

•5 

6 

Ol  .  45 

48.42 

.  oy 
5.55 

.ool 

.324 

NaCl. 

36 

25.22 

24.96 

24.98 

24.6 

44.88 

At    AA. 

7.92 
i  n  f\f\ 

.312 

OfkO 

NaNO3 

52.89 

52.84 

52.82 

86.6 

56.8 

33.61 

lU.DO 

17.02 

.  oUo 

.291 

29.86 
26.46 
20.00 
15.32 
10.97 

20.33 
23.48 
30.26 
36.09 
44.76 

.285 
.282 
.276 
.276 
1.291 

2.  Sat.  NaCl+Aq  treated  with  NaNO3. 
3.  Sat.  NaNO3+Aq  treated  with  NaCl.  , 
4.  Simultaneous  treatment  of  the  two  salts 
byH2O.    (Karsten.) 
6.  Excess  of  both  salts  -f-Aq  warmed  and 

(Engel,  C.  R.  1887,  104.  911.) 

cooled  to  20°.    (Rudorff,  B 

.  6.  484 

.) 

NITRATE,  SODIUM 


595 


Solubility  of  NaCl  with  addition  of  NaNO 
at  15.5°. 


Sp.  gr. 

100  ccm.  contain  in  g. 

NaCl 

H20 

NaNOs 

1.2025 

31.78 

88.47 

0.00 

1.2305 

27.89 

87.63 

7.53 

1.2580 

26.31 

86.25 

13.24 

1.2810 

23.98 

82.66 

21.58 

1.3090 

22.30 

80.42 

28.18 

1.3345 

20.40 

79.25 

33.80 

1.3465 

19.40 

77.37 

37.88 

1.3465 

19.67 

77.34 

37.64 

NaN03  separated  in  last  two  solutions. 

Solubility  of  NaNO3  with  addition  of 'NaCl 
at  15°. 


Sp.  gr. 


100  ccm.  contain  in  g. 


NaNOs 


H2O 


NaCl 


Solubility  in  NaCl+Aq  at  20°,  30°,  40°  and 
91°.  Tables  given  in  the  original  show  that 
each  salt  diminishes  the  solubility  of  the 
other.  (Leather,  'Mem.  Dept.  Agric.  India, 
1914,  3.  177;  Chem.  Soc.  1915,  108.  (2)  13.) 

See  also  under  NaCl. 

NaNO3+NaOH. 

Solubility  in  NaOH+Aq  at  0°.  NaNO8  = 
mols.  NaNOs  (in  mg.)  in  10  ccm.  of  solu- 
tion; Na2O  =  mols.  Na2O  (in  mg.)  in  10 
ccm.  of  solution. 


NaNOs 

Na2O 

NaNOs 
+Na20 

Sp.  gr. 

66.4 

0 

66.4 

.341 

62.5 

2.875 

65.375 

.338 

57.15 

6.1 

63.25 

.333 

47.5 

12.75 

60.25 

.327 

29.5 

26 

55.5 

.326 

17.5 

39 

56.5 

.332 

13.19 

45.875 

59.065 

.356 

6.05 

60.875 

66.925 

.401 

,3720 
.3645 
.3585 
.3530 
,3495 
,3485 
,3485 


1.3485 


62.38 
56.56 
52.09 
47.08 
42.66 
39.90 
38.73 
38.02 


74.82 
75.69 
75.71 
76.86 
76.96 
77.14 
77.15 
77.49 


0 

4.00 
7.24 
11.36 
15.33 
17.81 
18.97 
19.34 


(Engel,  Bull.  Soc.  (3)  6.  16.) 
Solubility  in  NaOH+Aq  at  0°. 


NaCl  separated  in  last  two  solutions. 
(Bodlander,  Z.  phys.  Ch.  7.  360.) 

Solubility  of  NaNO3  in  NaCl+Aq  at  15C 


Sp.  gr. 

G.  per  100  cc.  sat.  solution 

NaCl 

NaNOs 

H2O 

1.3720 

0 

62.38 

74.82 

1.3645 

4.0 

56.76 

75.69 

1.3585 

7.24 

52.09 

75.71 

1.3530 

11.36 

47.08 

76.86 

1.3495 

15.33 

42.66 

76.96 

1.3485 

17.81 

39.90 

77.14 

1.3485 

18.97* 

38.73* 

77.15 

1.3485 

19.34* 

38.02* 

77.49 

G.  per  100  cc.  solution 

Sp.  gr. 

NaOH 

NaNOs 

0.0 

56.50 

1.341 

2.30 

53.19 

1.338 

4.89 

48.63 

1  333 

10.21 

40.42 

1.327 

20.83 

25.10 

1.326 

31.25 

14.89 

1.332 

36.76 

11.22 

1.356 

48.75 

5.15 

1.401 

(Engel,  I.  c.) 

Easily  sol.  in  K2S04-fAq  without  pptn. 

Easily  sol.  in  Na2SO4+Aq  without  pptn. 

Sol.  in  MgSO4-f-Aq,  at  first  to  a  clear  solu- 
tion, but  afterwards  NaNO3  is  pptd. 

Very  sol.  in  sat.  CuSO4+Aq,  but  double 
sulphate  separates  out. 

Very  sol.  in  ZnSO4+Aq  with  pptn.  of 
double  sulphate.  (Karsten.) 

Solubility  of  NaNO3  in  Na2S2O3+Aq  at  t°. 


*  Solutions  sat.  with  both  salts. 
(Bodlander,  Z.  phys.  Ch.  1891,  7.  361.) 

Solubility  of  NaNO3+NaCl  (g.  in  100  g.  H2O) 
at  25°. 


NaNOs 

NaCl 

Solid  phase 

79.20 

68.38- 
56.56 
39.20 
20.17 

8.39 
16.32 
23.74 
27.56 
31.48 

NaNO3 

ii 

NaNO3+NaCl 

NaCl 

u 

25 


NaNOs 


33.31 

22.57 

4.22 


35.42 
25.40 
19.90 
18.02 
4.33 


Na2S2Os 


12.26 
23.41 

34.77 


12.72 
24.25 
31.81 
32.83 
40.50 


Solid  phase 


NaNOs 

"     +Na2S203,  5H20 
Na2S2O3,  5H2O 


NaNOs 

a 

"     +Na2S203,  5H20 
Na2S203,  5H20 


(Uyeda,  Mem.  Col.  Sc.  Kioto,  1910,  2.  245.) 


(Kremann  and  Rothmund,  Z.  anorg.  1914, 
86.  373.) 


596 


NITRATE,  SODIUM 


Very  sol.  in  liquid  NH3.  (Franklin,  Am. 
Ch.  J.  1898,  20.  829.) 

Easily  sol.  in  liquid  HF.  (Franklin,  Z. 
anorg.  1905,  46.  2.) 

Hydrazine  dissolves  26.6  pts.  NaNO3  at 
12.5-13°.  (de  Bruyn,  R.  t.  c.  1899,  18.  297.) 

100  pts.  alcohol  of  0.9  sp.  gr.  dissolve  10.5  pts.  NaNOs; 
0.872  sp.  gr.,  6  pts.;  0.834  sp.  gr.,  0.38  pt.;  insol.  in 
alcohol  of  0.817  sp.  gr.  (Kirwan.) 

100  pts.  alcohol  of  61.4%  by  weight  dissolve  21.2  pts. 
NaNOs  at  26°.  (Pohl,  W.  A.  B.  6.  600.) 

100  pts.  alcohol  of  62°  Tr.  dissolve  7.4  pts.  NaNOs  at 
19.5°. 

100  pts.  alcohol  of  93°  Tr.  dissolve  0.93  pt.  NaNOs  at 
19.5°.  (Wittstein.) 

100  pts.  alcohol  containing  %  alcohol  by 
weight  dissolve  pts.  NaNO3  at  15°,  or  100 
pts.  solution  contain  %  NaN03: 

10      20      30      40       60      80%  alcohol. 
65.3    48.8    35.5   25.8    11.4    2.8  pts.  NaNO3. 
39.5   32.8   26.2   20.5    10.2   2.7%  NaNO3. 

(Schiff.) 

100  pts.  wood-spirit  of  40%  dissolve  32.3 
pts.  NaNO3.  (Schiff,  A.  118.  365.) 


Solubility  in  alcohol  at  30°. 


Wt.  %  alcohol 
in  solvent 

G.  NaNOs  per  100  g. 

Solution 

Water 

0 

49.10 

96.45 

5 

46.41 

91.15 

10 

43.50 

85.55 

20 

37.42 

74.75 

30 

31.31 

65.10 

40 

25.14 

55.95 

50 

18.94 

46.75 

60 

12.97 

37.25 

70 

7.81 

28.25 

90 

1.21 

12.25 

(Taylor,  J.  phys.  Ch.  1897,  1.  723.) 


Solubility  in  ethyl  alcohol  at  25°. 

(Concentration  of  alcohol  in  g.  mol.  per 
1000  g.  H2O.) 


Solubility  in  alcohol  at  16.5°. 

Normality 

Solubilitv  in  1000 
g.  H20 

Mol.  solubility 

Sp.  gr. 

100  ccm.  contain  in  g. 

1 

2 

920 
908 
896 
870 

825 

.30 
.80 
60 
95 
35 

10.83 
10.70 
10.54 
10.24 
9.70 

Alcohol 

Water 

NaNOs 

1.3745 
1.3162 
1.2576 
.2140 
.1615 
.0855 
.0558 
.0050 
0.9420 
0.9030 
0.8610 

0 
6.16 
11.60 
16.49 
22.17 
32.22 
37.23 
43.98 
52.60 
60.00 
63.16 

75.25 
70.82 
68.10 
65.04 
61.67 
52.92 
48.50 
42.78 
32.13 
25.65 
21.31 

62.20 
54.64 
46.06 
39.87 
32.31 
23.41 
19.85 
13.74 
9.47 
4.65 
1.63 

(Armstrong  and  Eyre,  Proc,  R.  Soc.  1910  (A), 
84.  127.) 

Very  si.  sol.  in  acetone.    (Krug  and  M'El- 
roy,  J.  Anal.  Ch.  6.  184.) 

Solubility  of  NaNO3  in  acetone  at  40°. 

(Bodlander,  Z.  phys.  Ch.  7.  317.) 

100  pts.  absolute  methyl  alcohol  dissolve 
0.41  pt.  at  25°. 
100  pts.   absolute   ethyl   alcohol  dissolve 
0.036  pt.  at  25°.    (de  Bruyn,  Z.  phys.  Ch.  10. 
783.) 
Solubility  in  alcohol  at  40°. 

Wt.  %  acetone 

G.  NaNOs  per  100  g. 

acetone  +Aq 

0.0 
8.47 
16.8 
25.2 
34.3 
44.1 
53.9 
64.8 
76.0 
87.6 

105 
91.2 
78.3 
66.4 
57.9 
46.2 
32.8 
23.0 
10.8 
3.2 

Wt.  %  alcohol 

G.  NaNOs  per  100  g. 
alcohol  +Aq. 

0 
8.22 
17.4 
26.0 
36.0 
42.8 
55.3 
65.1 
77.0 
87.2 

104.5 
90.8 
73.3 
61.6 
48.4 
40.6 
27.1 
18.1 
9.4 
4.2 

(Bathrick 

,  J.  phys.  Ch.  1896,  1.  }62.) 

(Bathrick,  J.  phys.  Ch.  1896, 

1.  162.) 

NITRATE,  STRONTIUM 


597 


Solubility  of  NaNO3  in  acetone  at  30°. 

100  pts.   H2O   dissolve  at  0°,    39.5   pts. 
Sr(NO3)2  (Mulder);  at  0°,  40.16  pts.  Sr(N03)2 

G.  NaNOs  per  100  g. 

(Poggiale);  at  0°,  43.1  pts.  Sr(NO3)2  (Krem- 

Wt.  %  acetone 

ers);  at  100°,  101.1  pts.  Sr(NO3)2  (Mulder); 

in  solvent 

Solution 

Water 

at  100°,  106.5  pts.  8r(NOt)l  (Kremers,  Pogg. 

92.  499);  at  100°,  119.25  pts.  Sr(NO3)2  (Pog- 

0 

49.10 

96.45 

giale). 

5 

46.96 

93.20 

9.09 
20 

45.11 
40.10 

90.40 
83.70 

Solubility  in  100  pts.  H2O  at  t°. 

30 

35.08 

77.20 

Pts. 

Pts. 

Pts. 

40 

29.80 

CIA    q/i 

70.75 

t° 

Sr(NOa)2 

t° 

Sr(N03)2 

t 

Sr(NOi)« 

60 

A'*.  .  OT: 

18.55 

59  '.95 

0 

39.5 

36 

90.7 

73 

96.0 

70 

13.15 

50.50 

1 

41.2 

37 

90.8 

74 

96.2 

80 

7.10 

38.20 

2 

42.8 

38 

91.0 

75 

96.4 

90 

1.98 

20.20 

3 

44.3 

39 

91.1 

76 

96.5 

4 

45  8 

40 

01     Q 

77 

Qfi  7 

(Taylor,  Z.  phys.  Ch.  1897,  2.^723.) 

5 
6 

47^3 

48.8 

TrU 

41 
42 

*7X  -  O 

91.4 
91.5 

1    I 

78 
79 

t/U  •  * 

96.8 
97.0 

7 

50.3 

43 

91.6 

80 

97.2 

8 

51.8 

44 

91.8 

81 

97.4 

Sol.  in  glycerine. 
Insol.   in   ethylamine.      (Shinn,    J.   phys. 

9 
10 

53.4 
54.9 

45 
46 

91.9 
92.1 

82 
83 

97.5 
97.7 

Chem.  1907,  11.  538.) 
Insol.  in  methyl  acetate.     (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.     (Naumann, 

11 
12 
13 

56.5 
,58.0 
59.6 

47 
48 
49 

92.2 
92.3 
92.5 

84 
85 
86 

97.9 
98.0 
98.2 

B.  1910,  43.  314.) 
Insol.  in  benzonitrile.    (Naumann,  B.  1914, 

14 
15 

61.2 
62.8 

50 
51 

92.6 
92.8 

87 
88 

98.4 

47.  1370.) 

16 

64.4 

52 

92.9 

89 

98^8 

17 

66.0 

53 

93.1 

90 

99.0 

18 

67.6 

54 

93.2 

91 

99.2 

Sodium     thorium     nitrate,     NaTh(NOs)6  + 

19 

69.2 

55 

93.4 

92 

99.4 

9H20. 

20 

70.8 

56 

93.5 

93 

99.6 

Hydroscopic;  sol.  in  dil.  HN03  and  Aq. 
(Meyer,  Z.  anorg.  1901,  27.  381.) 

21 

22 
23 

72.5 
74.1 

75.8 

57 

58 
59 

93.6 
93.8 
93.9 

94 
95 

96 

99.8 
100.0 
100.2 

24 

77.4 

60 

94.0 

97 

100.4 

Sodium  nitrate  sulphate,  NaNO3,  Na2SO4-f- 

25 
26 

79.0 

80.7 

61 

62 

94.2 
94.3 

98 
99 

100.6 
100.9 

Sol.  in  H2O.    (Marignac,  Ann.  Min.  (5)  12. 

27 

28 

82.4 
84.1 

63 
64 

94.5 
94.6 

100 
101 

101.1 
101.3 

44.) 

29 

85  8 

65 

94  8 

102 

101.6 

+H2O.    Min.  Darapskite. 

30 

87.6 

66 

94^9 

103 

101.8 

31 

89.5 

67 

95.1 

104 

102.0 

31.3 

90.0 

68 

95.2 

105 

102.3 

Sodium  nitrate  tungstosilicate,  3Na4Wi2Si040. 
4NaNO3-f45H2O. 

32 
33 

90.2 
90.3 

69 
70 

95.4 
95.6 

106 
107 

102.5 
102.7 

(Wyruboff,  Chem.  Soc.  1897,  72.  (2)  174.) 

34 

90.5 

71 

95.7 

107.9 

102.9 

35 

90.6 

72 

95.9 

Strontium  nitrate,  Sr(NO3)2. 

Sol.  in  5  pts.  cold,  and  0.5  pt.  boiling  H2O.  (Dumas.) 
"  2  "  "  0.5  "  "  (Wittstein.) 

"  2  "  at  18.75°.  (Abl.) 

100  pts.  sat.  Sr(NOs)2+Aq  at  19-20°  contain  45.49 
pts.  Sr(NOs)2.  (v.  Hauer,  J.  pr.  98.  137.) 


1  pt.  Sr(NOs)2  dissolves  in  pts.  H2O  at  t°. 


t 

Pts.  H20 

t° 

Pts.  H20 

t° 

Pts.  H20 

0 
10 

2.32 
1.73 

25 
50 

1.10 
1.02 

75 
100 

0.99 
0.94 

(Kremers,  Pogg.  92.  499.) 

(Mulder,  Scheik.  Verhandel.  1864.  114.) 

Sat.  Sr(NO3)2-HAq  contains  at: 
—6°       +14°     20°        32° 
24.5      35.9      39.8       46.9%  SrNO3, 

53°        56°        76°        94°       110° 
47.2       47.8       49.1       50.4       50.2%  SrNO3. 

(fitard,  A.  ch.  1894,  (7)  2.  528.) 

79.27  g.  anhydrous  Sr(N03)2  are  sol.  in 
100  g.  H2O  at  25°.  (Parsons  and  Carson,  J. 
Am.  Chem.  Soc.  1910,  32.  1385.) 


NITRATE,  SODIUM 


Solubility  of  Sr(NO3)2  in  H2O  at  t°. 


t° 

G.  Sr(NO3)2in 
100  g.  H20 

Sp.  gr. 

0.58 

40.124 

1.2856 

14.71 

60.867 

1.3938 

26.40 

82.052 

.4883 

29.06 

87.648 

.5110 

30.28 

88.577 

.5144 

32.58 

88.943 

.5141 

39.74 

90.086 

.5128 

47.73 

01.446 

.5115 

61.34 

93.856 

1.5105 

68.96 

95.576 

1.5106 

78.98 

97.865 

1.5109 

88.94 

100.136 

1.5117 

(Berkeley  and  Appleby,  Proc.  R.  Soc.  1911, 
(A)  85.  503.) 

100  g.  of  the  sat.  solution  contain  at  20°, 
41.43  g.  Sr(NO3)2.  (Findlay,  Chem.  Soc. 
1914,  106.  782.) 

Sp.  gr.  of  Sr(NO3)2+Aq  at  19.5°. 


Sr(N°O3)2 

Sp.  gr. 

Sr(N°Os)2 

Sp.  gr. 

1 

.009 

21 

1.192 

2 

.017 

22 

1.202 

3 

.025 

23 

1.213 

4 

.034 

24 

.223 

5 

.041 

25 

.233 

6 

.049 

26 

.246 

7 

1.059 

27 

.257 

8 

1.068 

28 

.268 

9 

1.076 

29 

.280 

10 

1.085 

30 

.292 

11 

1.095 

31 

.304 

12 

1.103 

32 

.316 

13 

1.113 

33 

.330 

14 

1.122 

34 

1.340 

15 

.131 

35 

1.354 

16 

.140 

36 

1.367 

17 

.150 

37 

1.381 

18 

.160 

38 

1.395 

19 

.170 

39 

1.410 

20 

.181 

40 

1.422 

(Kremers.  calculated  by  Gerlach,  Z.  anal.  8. 

286.) 

Sp.  gr.  of  Sr(NO3)2+Aq  at  23.4°.  a=no.  of 
grms.  X1A  mol.  wt.  dissolved  in  1000 
grms.  H2O;  b  =  sp.  gr.  if  a  is  Sr(NO3)2, 
4H2O,  Yi  mol.  wt.  =  142;  c  =  sp.  gr.  if  a  is 
Sr(N03)2,  ^mol.  wt.  =  106. 


a 

b 

c 

a 

b 

c 

1 

2 

3 

4 

1.078 
1.146 
1.205 
1.257 

1.081 
1.155 
1.224 

1.284 

5 
6 

7 

1.303 
1.345 
1.383 

1.350 
1.407 

(Favre  and  Valson,  C.  R.  79.  968.) 

Sp.  gr.  of  Sr(NO3)2-f  Aq  at  17.5°. 


%  Sr(NO3)2 


10 
20 
30 


Sp.  gr. 


1.083 
1.180 
1.294 


%  Sr(N03); 


40 

Sat.  sol. 


Sp.  gr. 


1.422 
1.52 


(Gerlach,  Z.  anal.  27.  283.) 


Sp.  gr.  of  Sr(NO3)2+Aq  at  t°. 


14.0° 
14.3° 
14.5° 
14.5° 
14.5° 
14.4° 


%  Sr(NO3)2 


5 
10 
15 
20 
25 
34.33 


Sp.  gr. 


1.0420 
1.0859 
1.1319 
1.1816 
1.2364 
1.3470 


(Long,  W.  Ann.  1880,  11.  39.) 


Sp.  gr.  of  Sr(NO3)2+Aq  at  room  temp, 
containing: 

10.29       21.19  .     32.61%  Sr(NO3)2. 
1.0885      1.124      1.3067 

(Wagner,  W.  Ann.  1883,  18.  266.) 


Sp.  gr.  of  Sr(NO3)2+Aq  at  25°. 


Concentration  of 
Sr(NO3)2+Aq 

Sp.  gr. 

1-normal 

Vr-       " 

V4-     " 

Vs-       " 

1.0822 
1.0419 
1.0208 
1.0104 

(Wagner,  Z.  phys.  Ch.  1890,  5.  40.) 


Sr(N03)2+Aq  containing  10.50%  Sr(N03)2 
has  sp.gr  20720°  =  1.0905. 

Sr(NO3)2+Aq  containing  25.51%  Sr(N03)2 
has  sp.  gr.  20°/20°  =  1.2440. 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  279.) 


Sp.  gr.  of  Sr(NO3)2+Aq  at  20°  containing 
M  g.  mols.  of  salt  per  liter. 
M         0.01          0.025        0.05          0.075 
Sp.  gr.  1.001525  1.004207  1.008391  1.012646 


M         0.10          0.25 
Sp.  gr.  1.016834  1.04201 


0.50          0.75 
1.08312     1.12386 


M         1.00 
Sp.  gr.  1.16354 

(Jones  and  Pearce,  Am.  Qh.  J.  1907,  38.  705.) 


NITRATE,  TELLURIUM 


599 


B.-pt.    of    Sr(NO3)2+Aq,     containing    pts 
Sr(NO3)2  to  100  pts.  H2O. 

the  solutions  which  contain  small  amounts  of 
alcohol. 

(D'Ans  and  Siegler,  Z.  phys.  Ch.  1913,  82.  39.) 

Not  .completely    insol.    in    boiling    amyl 
alcohol,    30    ccm.    dissolving    about    1    mg. 
(Browning,  Sill.  Am.  J.  143.  52.) 
Perfectly   anhydrous  Sr(NO3)2  is   sol.    in 
83044    pts.    absolute    ether-alcohol    (1:1). 
(Fresenius,  Z.  anal.  32.  190.) 

Solubility  in  organic  solvents. 

B"P*'            Sr(N03)2             B"P*- 

Pts. 

Sr(NOs)2 

100.5°.         12                104° 
101               24                104.5 
101.5           34.8            105 
102               45                105.5 
102.5           54.4            106 
103               63.6            106.3 
103.5           72.6 

81.4 
89.6 
97.6 
105 
112.2 
116.5 

(Gerlach,  Z.  anal.  26.  448.) 

Sat.  Sr(NO,),+Aq  boils  at  106.8°,  and  con- 
tains 112.9  pts.  salt  to  100  pts.  H2O.    (Grif- 
fiths.) 
Sat.    Sr(NO3)2-hAq    boils    at    107.5-108° 
(Kremers);  107.9°  (Mulder). 
Sat.  Sr(NO3)2+Aq  forms  a  crust  at  106.3°, 
and  contains  116.5  pts.  Sr(NO3)2  to  100  pts. 
H2O;    highest    temp,    observed    was    107°. 
(Gerlach,  Z.  anal.  26.  427.) 
Very  si.  sol.  in  cone.  HNO3  or  HCl+Aq. 
(Wurtz.) 
Insol.  in  HNO3+Aq.     (Schultz,  Zeit.  Ch. 
(2)  6.  537.) 

Solubility  in  Sr(OH)2,  8H2O+Aq  at  25°. 

Solvent                           %  Sr(N03)2  in  the 
solution  at  25° 

Methyl  alcohol                         1  .  26 
Ethyl  alcohol                           0.02 
Propyl  alcohol                          0  .  02 
Isobutyl  alcohol                      0.01 
Amyl  alcohol                            0  .  00& 
Acetone                                    0.02 

(D'Ans  and  Siegler,  Z.  phys.  Ch.  1913,  82.  44.) 

Insol.  in  methyl  acetate.     (Naumann.  B. 
1909,  42.  3790.) 
Insol.  in  benzonitrile.    (Naumann,  B.  1914, 
.47.  1370.) 
Sol.  in  acetone.    (Eidmann,  C.  C.  1899.  II, 
1014.) 
Difficultly  sol.  in  acetone.    (Naumann,  B 
1904,  37.  4328.) 
The  composition  of  the  hydrates  formed 
by  Sr(NO3)2  at  different  dilutions  is  calcu- 
lated from  determinations  of  the  lowering  of 
the  fr.-pt.  produced  by  Sr(NO3)2  and  of  the 
conductivity  and  sp.  gr.  of  Sr(NO3)2+Aq. 
(Jones,  Am.  Ch.  J.  1905,  34.  305.) 
+4H2O.    Efflorescent. 

Solubility  in  ethyl  alcohol  +Aq  at  25°. 

G.  SrO  as 
Sp.  gr.  25°/25°      Sr(OH)  2  in  100  g. 
H20 

G.  Sr(NO3)2  in 
100  g.  H20 

1.492                  0.38 
1.494                  0.78 

79.47 

80.83 

(Parsons,  J.  Am.  Chem.  Soc.  1910,  32.  1388.) 

Very  sol.  in  liquid  NH3.     (Franklin,  Am. 
Ch.  J.  1898,  20.  829.) 
Sol.  in  8500  pts.  absolute  alcohol.    Sol.  in 
60,000  pts.  of  a  mixture  of  1  pt.  ether  and  1 
pt.  alcohol.    (Rose,  Pogg.  110.  296.) 
Sol.  in  4189  pts.  abs.  alcohol  and  in  199.87 
pts.  ordinary  rectified  spirits.    (Hill,  Pharm. 
J.  1888  (3)  19.  420.) 

Solubility  in  ethyl  alcohol  +Aq  at  25°. 

%  C2H6OH  in 
the  solvent 

%  C2H6OH  in        %  Sr(NO3)2  in 
the  solution            the  solution 

0 
4 
6 
10.8 
16.0 
20 

0                      44.25 
1.7                  42.8 
2.6                  42.1 
4.95                40.4 
7.95                37.6 
12.35                34.3 

%  C2H6OH  in        %  C2H5OH  in 
the  solvent              the  solution 

%  Sr(NOs)2  in 
the  solution 

99.4                   99.38 
79.2                   77.15 
59.9                   53.6 
40.65                 32.35 
20.6                   13.8 
18.8                   12.35 
16.25                 10.45 
15.05                   9.5 
10.0                     6.0 
6.0                     3.45 
0                        0 

0.02 
2.60 
10.5 
20.5 
33.2 
34.3 
35.7 
36.7 
40.05 
42.7 
46.6 

(D'Ans  and  Siegler,  Z.  phys.  Ch.  1913,  82.  39.) 

Tellurium    nitrate,    basic,    4TeO2,    N2O6-h 
1^H20. 
Very  hygroscopic.   Easily  decomp.  by  H2O. 
Sol.  in  HNO3+Aq,  but  more  sol.  when  dil. 
than  cone.    (Klein  and  Morel,  Bull.  Soc.  (2) 
43.  205.) 

Tellurium  nitrate,  TeNO3. 

Sol.  in  acetone.    (Eidmann,  C.  C.  1899.  II, 
1014.) 

Sr(NO3)2  is  the  solid  phase  in  the  solutions 
which  are  rich  in  alcohol;  Sr(NO3)2-h4H2O  in 

600 


NITRATE,  TERBIUM 


Terbium  nitrate,  Tb(NO8)8+6H2O. 

Sol.  in  H2O.    Sol.  in  alcohol.    (Urbain,  C. 
R.  1908,  146.  128.) 

Thallous  nitrate,  T1NO3. 

1  pt.  T1NO3  dissolves,  according  to  C  = 
Crookes;  L  =  Lamy: 

at  15°      18°     58°     107° 
in  9.4     10.3    2.3     0.17  pts.  H2O. 
C       L        L       L 

Sat.  TINOs+Aq  contains  at: 
3.5°        18°        32°        58°        95° 
4.2          8.8        13.2       30.4       74.5%  T1NO3 

107°       135°       145°       150°       155° 
85          95        95.2       96.5         97%  T1NO3. 
(fitard,  A.  ch.  1894,  (7)  2.  527.) 


Solubility  in  H2O  at  t° 


Thallous  thallic  nitrate,  2T1NO3,  T1(NO8)«. 

Decomp.  by  H2O.  (Wells,  Am.  Ch.  J. 
1901,  26.  278.) 

Thallous  uranyl  nitrate,  T1(UO2)(NO3)3. 

Decomp.  in  moist  air.  Decomp.  by  H2O. 
(Meyer,  B.  1903,  36.  4058.) 

Thorium  nitrate,  ThO2,  2N2O5+6H2O. 

Crystallized.  SI.  hydroscopic.  (Fukse, 
Zeit.  angew.  Ch.  1897,  10.  116.) 

+12H2O.  Very  deliquescent,  and  sol.  in 
H2O  and  alcohol. 

Difficultly  sol.  in  acetone.  (Naumann,  B. 
1904,  37.  4328.) 

Thorium  zinc  nitrate,  ZnTh(NO3)6+8H2O. 

Sol.  in  HNO3;  very  hydroscopic.  (Meyer, 
Z.  anorg.  1901,  27.  386.) 


t° 

G.  TINOs 
in  100  g.  HzO 

g.  mol.  TINOs 
in  1  1. 

inuiium  nitrate,  im2iiNU3;6-t-»rL2u. 
Deliquescent.    Can  readily  be  cryst.  from 
HNO3     (James,  J.  Am  Chem.  Soc.  1911,  33. 

0 

3.91 

0.149 

1344.)' 

10 

6.22 

0.230 

20 

9.55 

0.357 

Tin  (stannous)  nitrate,  basic,  2SnO,  N205. 

25 

.... 

0.433 

Difficultly  sol.  with  partial  decomp.  in  H2O. 

30 

14.3 

0.522 

(Weber,  J.  pr.  (2),  26.  121.) 

40 

20.9 

0.755 

50 

30.4 

1.07 

Tin  (stannous)  nitrate,  Sn(N03)2-f-20H2O. 

60 
70 

46.2 
69.5 

1.58 
2.29 

Deliquescent,  and  easily  decomp.    (Weber, 
J.  pr.  (2)  26.  121.) 

80 

111 

3.40 

90 
100 

200 
414 

5.32 
8.29 

Tin  (stannic)  nitrate,  basic,  4SnO2,  N206+ 

4.TT  O 

105 

594 

10.25 

^t£l2vy. 

(Thomas,  Bull.  Soc.  1896  (3)  15.  312.) 

(Berkeley,  Trans.  Rov. 

Soc.  1904,  203.  A, 

211. 

Tin  (stannic)  nitrate,  Sn(N03)4. 

Sol.  in  H20,  but  decomp.  very  soon  on 

Sp.  gr.  of  TlNO8+Aq  at  25°. 

standing.   Stable  in  presence  of  cone.  HNO3  + 

Mf\4-       C\f\O          Vv1l4-        ^-1  ^rt^-iw*-^           n4-        1  AAO                 f*\/f  r\-n4-n 

Concentration  of 
TINOs+Aq 

Sp.  gr. 

at  yu  ,  out  aecomp.  at  luu  .     ^ivionte- 
martini,  Gazz.  ch.  it.  22.  384.) 
Insol.  in  moderately  cone.  HNO3;  readily 

1/4-normal 

1.0562 

decomp.  by  H2O.     (Engel,  C.  R.  1897,  125. 

T1  f\  \ 

Vs-      " 

1.0283 

710.) 

(Wagner,  Z.  phys.  Ch.  1890,  6.  40.) 

Solubility  of  T1N08+KN08.    (See  KN03.) 
Insol.  in  alcohol.    (Lamy.) 
Sol.  in  acetone.    (Eidmann,  Dissert.  1899; 
Naumann,  B.  1904,  37.  4328.) 

Thallous  hydrogen  nitrate,  T1NO3,  2HNO3. 
(Wells,  Am.  Ch.  J.  1901,  26.  273.) 
T1N03,  3HN03.    (Ditte.) 

ThalUc  nitrate,  Tl(N08)3-f-3H2O. 

Effloresces  in  the  air.  (Meyer,  Z.  anorg. 
1900,  24.  361.) 

+6H2O,  or  8H2O.  Deliquescent.  Sol.  in 
H20. 


Titanium  nitrate,  5TiO2,  N2O6+6H2O. 

Sol.   to  a  slight  milkiness  in  cold  H2O. 
Decomp.  on  boiling.    (Merz,  J.  pr.  99.  157.) 

Uranyl  nitrate,  basic. 

Sol.  in  H20.    (Ordway,  Sill.  Am.  J.  (2)  26. 
209.) 

Uranyl  nitrate,  UO2(NO8)2. 

+H2O.     (de  Forcrand,  C.  R.  1913,  166. 
1046.) 

Sol.  in  fuming  HNO3  from  which  it  can 
be  cryst. 

+2H2O.    52.39%  is  sol.  in  dry  ether  at   7°. 
54.25%  "   "    "    "      "       "  10°. 
(Lebeau,  Bull.  Soc.  1911,  (4)  9.  300.) 


NITRATE,  URANYL 


601 


+2H20.    (Vasilieff,  C.  C.  1910,  II.  1527.) 
+3H2O.    Mpt.  121.5°.    (Vasilieff.) 
Cryst.  out  of  hot  HNO3+Aq.    (Ditte.) 
100  pts.  HNO3  dissolve  39  pts.   at   14°. 
(Ditte,  A.  ch.  1879,  (5)  18.  337.) 
+4H2O.    (de  Coninck,  C.  C.  1901,  1.  1354.) 
+6H2O.    Deliquescent  in  moist,  and  efflo- 
rescent in  dry  air.    Sol.  in  0.5  pt.  cold  H2O,  in 
0.3  pt.  absolute  alcohol,  and  in  4.0  pts.  ether. 
(Bucholz.) 
Melts  in  crystal  H2O  at  59.4°.    (Ordway.) 
1  pt.  is  sol.  in  2  pts.  H2O  at  12.9°-14.2°. 
(de  Coninck,  C.  R.  1900,  131.  1220.) 

Solubility  in  H2O  at  t°. 

Sp.  gr.  of  solution  in  H2S04+Aq. 

Pts.  of  salt  in 
100  pts.  H2SO4 
sp.  gr.  1.138 

1  pt.     2  pts.    3  pts.    4  pts.    5  pts. 

Temp. 

11.2°     11.8°     10.7°     12.0°     11.4° 

Sp.  gr.  of  solution 

1  .  1427  1  .  1450  1  .  1511  1  .  1540  1  .  1576 

(de  Coninck.) 

Very   sol.   in   dil.   HBr   and   selenic   acid 
(d  =  1.4).     Sol.  in  cone.  H2SO4,  HNO3,  dil. 
SCI  and  less  sol.  in  cone.  HC1.    (de  Coninck, 
C.  R.  1900,  131.  1220.) 

Sp.  gr.  of  solution  in  HBr+Aq  of  sp.  gr.  1.21. 

t° 

%  by  wt.  UO2(NOs)2,  6H2O 

Sp.  gr. 

%  salt  dissolved 

54.90 
58.00 
62.13 
63.01 
67.36 
72.83 
78.05 
82.96 
86.32 

—18.1 
—12.1 
—  2.2 
0 
+  12.3 
25.6 
36.7 
45.2 
71.8 

1.2122                                 1 
1.2168                                 2 
1.2198                                 3 
1.2250                                 4 
1.2305                                 5 

(de  Coninck,  Belg.  Acad.  Bull.  1901.  222.) 

Insol.  in  KOH+Aq,  NaOH+Aq  or  NH4OH 
+Aq.    Sol.  in  lime  water,    (de  Coninck,  C.  R. 
1900,  131.  1220.) 
SI.  attacked  by  liquid  NH3.     (Gore,  Am. 
Ch.  J.  1898,  20.  830.) 
At  15°,  uranyl  nitrate  is  sol.  in  comm. 
methyl  alcohol,  dil.  and  cone,  ethyl  alcohol, 
propyl   and  isobutyl   alcohol,    comm.    amyl 
alcohol,   acetone,   ether,    ethyl   acetate,   dil. 
and  cone,  formic  acid  and  dil.  acetic  acid;  si. 
sol.  in  comm.  essence  of  terebenthine;  insol. 
in  benzene  (cryst.),  comm.  toluene  and  xylene, 
ligroin,  CHC13,  glycerine  and  CS2.    (de  Con- 
inck, C.  R.  1900,  131.  1220.) 
1  pt.  is  sol.  in  55  pts.  methyl  alcohol  at  ca. 
11.8°. 
1  pt.  is  sol.  in  30  pts.  ethyl  alcohol  (85°)  at 
ca.  12.9°. 
1  pt.  is  sol.  in  65  pts.  acetone  at  ca.  12.0°. 
1  pt.  is  sol.  in  5.6  pts.  acetic  acid  (d  =  1.035) 
at  ca.  14.25°. 
(de  Coninck,  C.  R.  1900,  131.  1304.) 

1  pt.  sol.  in  23.5  pts.  methyl  alcohol  at  11.2°. 
1  "     "   "16.0  "    ether                 "  11.9°. 
1  "      "    "18.4  "    ethyl  acetate     "  10.3°. 
1  "     "   "   5.3   "    cone,  formic  acid  at 
15.1°. 

(Vasilieff,  J.  Russ.  Phys.  Chem.  Soc.  1910, 
42.  570.) 

Sp.  gr.  of  (UO2)(NO3)2+Aq  at  t°. 

t° 

%  salt 

Sp.  gr. 

11.5 
12.4 
15.1 
14.1 
16.7 
14.1 
15.7 
15.2 
16.5 
15.2 
13.7 
11.5 
14.5 
11.3 
12.5 
13.2 

1 

2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 

1.0049 
1.0096 
1.01401 
1.0187 
1.0230 
1.8281 
1.0236 
1.0378 
1.0410 
1.0462 
1.0504 
1.0550 
1.0594 
1.0643 
1.0680 
1.0718 

(de  Coninck,  C. 
Sp.  gr.  of  a  sat.  aq 

R.  1900,  131.  1219.) 
.solution  =  1.7536  at  17°, 

containing  54.77%  UO2(NO3)2. 

Sp.  gr.  =  1.0257  when  2.80%  U02(NO3)2 
is  present.    (Vassiliev,  C.  C.  1912.  I,  1430.) 


(de  Coninck,  C.  R.  1901,  132.  91.) 

Sp.  gr.  of  solution  in  comm.  methyl  alcohol 
att°. 


Sp.  gr.  of  solution  in  HNOa+Aq. 

Pts.  of  salt  in 
100  pts.  HNO, 
sp.  gr.  1.153 

1 

2 

3 

4 

5 

Temp. 

11.0° 

11.8° 

11.3° 

12.0° 

11.6° 

Sp.  gr.  of  the  so- 
lution 

1.1585 

1.1614 

1.1663 

1  .  1698 

1.1751 

(de  Coninck,  C.  R.  1901,  132.  90.) 

t° 

%  salt 

Sp.  gr.  referred 
to  H2O 

11 

12.9 
12.2 
10.7 

12.8 

1 

2 
3 

4 
5 

0.8902 
0.8938 
0.9003 
0.9068 
0.9108 

(de  Coninck,  C.  R.  1900,  131.  1304.) 


602 


NITRATE  AMMONIA,  URANYL 


Sp.  gr.  of  solution  in  ethyl  alcohol  (85°)  at  t°. 
d2=sp.  gr.  referred  to  alcohol. 
di=sp.  gr.  referred  to  H2O. 

Ytterbium  nitrate. 
Very  sol.  in  H2O. 
+3H2O.     Ppt.     (Cleve,   Z.   anorg.    1902, 
32.  140.) 
+4H2O.    (Cleve.) 

Yttrium  nitrate,  basic,  2Y203,  3N2O5+9H2O. 
Deliquescent  in  moist  air.     Decomp.  by 
cold  or  boiling  H2O.     Sol.  in  a  solution  of 
yttrium  nitrate  without  decomp.    (Bahr  and 
Bunsen.  A.  137.  1.) 

t° 

%  salt 

di 

d2 

11.9 
12.2 
11.6 
13.1 
11.7 

1 

2 
3 
4 
5 

0.8918 
0.8979 
0.9023 
0.9056 
0.9131 

1.0060 
1.0127 
1.0177 
1.0227 
1.0280 

(de  Coninck,  C.  R.  1900,  131.  1219.) 

Sp.  gr.  of  solution  in  acetic  acid  (d  =  1.055) 

att°. 

di  =  sp,  gr.  referred  to  H2O. 
d2=sp.  gr.  referred  to  acetic  acid. 


t° 

%  salt 

di 

d2 

14.0 

1 

1.0387 

1.0034 

13.8 

2 

1.0434 

1.0080 

14.8 

3 

1.0469 

1.0100 

16.9 

4 

1.0505 

1.0148 

14.6 

5 

1.0564 

1.0205 

10.4 

6 

1.0626 

1.0265 

11.7 

7 

1.0662 

1.0300 

(de  Coninck,  C.  R.  1900,  131.  1304.) 

When  excess  of  UO2(NO3)2  is  shaken  with 
ether  at  7°,  two  layers  are  formed,  the  ether 
layer  containing  59  g.  salt  per  100  g.  solution 
and  the  aqueous  layer  62.5  g.  salt  per  100  g. 
solution.  (Lebeau,  C.  R.  1911,  152.  440.) 

Sol.  in  nearly  all  proportions  in  glycerine. 
(Postans,  Pharm.  J.  1883,  (3)  13.  752.) 

Sol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (ISaumann, 
B.  1904,  37.  3601.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899. 
II,  1014;  Naumann,  B.  1904,  37.  4328.) 

+18H2O.  Sat.  aq.  solution  has  D17°/17°  = 
1.7536.  (Vasilieff,  J.  Russ.  phys.  Chem.  Soc. 
1911,  43.  1183.) 

TJranyl   nitrate   ammonia,    (UO2)(NO3)2, 

2NH8. 
(v.  Unruh,  Dissert.  1909.) 

(UO2)(NO3)2,  3NH3.     (v.  Unruh.) 
(UO2)(NO3)2,  4NH3.    (v.  Unruh.) 

Uranyl     nitrate     phosphate,     UO2H4(PO4)2, 

UO2(NO3)2  +  14H2O. 

Easily  sol.  in  warm  H2O,  with  gradual 
decomp.  Easily  sol.  in  HN03,  HC1,  or 
H2SO4+Aq.  Sol.  in  acetic  acid  with  decomp. 
(Heintz,  A.  151.  216.) 


Divanadyl  nitrate  (?). 

Known    only   in    solution, 
evaporation. 

Ytterbium  nitrate,  basic. 
Easily  sol.  in  H2O. 


Decomp.    on 


Yttrium  nitrate,  Y(NO3)3+6H2O. 

Easily  sol.  in  H2O,  alcohol,  or  ether. 
(Cleve.) 

141.6  grams  are  sol.  in  100  grams  H2O  at 
25°.  (James,  J.  Am.  Chem.  Soc.  1910,  32. 
876.) 

Zinc  nitrate,  basic,  8ZnO,  N2O6+2H2O. 

Insol.  in  H2O.    (Grouvelle,  A.  ch.  19.  137.) 

6ZnO,  N2O6+8H2O=Zn(NO3)2,  5Zn(OH)2 
+3H2O.  (Bertels,  J.  B.  1784.  274.) 

5ZnO,  N2O5+5^H2O.  Insol.  in  cold, 
somewhat  sol.  in  hot  H2O.  (Havermann.) 

+6H2O.  Slowly  decomp.  by  cold  H2O. 
(Rousseau  and  Tite.) 

9ZnO,  2N2O6.  Decomp.  by  H2O.  (Vogel 
and  Reischauer,  N.  Jahrb.  Pharm.  11.  137.) 

4ZnO,  N2O5+2H2O.     (Schindler.) 

+3H2O.  (Ordway,  Sill.  Am.  J.  (2)  32.  14; 
Gerhardt,  J.  Pharm.  (3)  12.  61.) 

Insol.  in  H2O;  sol.  in  dil.  acids.  (Athan- 
asesco,  Bull.  Soc.  1896,  15.  1080.) 

2ZnO,  N2O6+3H2O.  Decomp.  by  H2O,  and 
slowly  by  alcohol.  (Wells,  Am.  Ch.  J.  9.  304.) 

7ZnO,  4N205+14H2O=4Zn(NO3)2, 
3Zn(OH)2+llH2O.     (Bertels.) 

Zinc  nitrate,  Zn(NO3)2. 

Very  deliquescent.  Easily  sol.  in  H2O  or 
alcohol. 

Sp.  gr.  of  Zn(NO3)2+Aq.  F.  =  according  to 
Franz  (J.  pr.  (2)  5.  274)  at  17.5°;  O.  =  accord- 
ing to  Oudemans  (Z.  anal.  7.  410)  at  14°: 

5  10  15%Zn(NO3)2, 

F.        1.0496        1.0968       1.1476 
O.        1.0425        1.087         1.1355 


20 

1.2024 
1.1875 


25 

1.2640 
1.245 


30%Zn(N03)2, 
1.3268 
1.305 

50%Zn(NO3)2. 
1.5984 


35            40            45 
F.  1.906     1.4572     1.5258 
O 

Calculated  for  Zn(NO3)2+6H2O: 

10  20  30          40        50%  salt. 

1.05361    1.1131    1.1782    1.2496    1.3292 
(Oudemans.) 

Zn(NO3)2+Aq  when  heated  soon  decom- 
poses, with  formation  of  an  insol.  basic  salt. 
(Ordway.) 


NITRIC  OXIDE 


603 


Sp.  gr.  of  Zn(NO3)2+Aq  at  room  temp, 
containing: 

15.955      30.626      44.5%  Zn(NO3)2. 
1.1155       1.2291       1.4367 

(Wagner,  W.  Ann.  1883, 18.  270.) 


Very  easily  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  830.) 

+  1^H2O.  100  pts.  HNO3  dissolve  28 
pts.  at  13°;  55  pts.  at  55°.  (Ditte,  A.  ch. 
1879,  (5)  18.  335.) 

r}-2H2O.    (Vasilieff,  C.  C.  1909,  II.  1966.) 

+3H20. 

Solubility  in  H2O. 

Sat.  solution  contains  at: 
37°      40°      41°      43°        45.5°mpt. 
66.38  67.42  68.21  69.26  77.77%  Zn(NO3)2. 
(Funk,  Z.  anorg.  1899,  20.  401.) 


+6H2O. 

Solubility  in  H2O. 

Sat.  solution  contains  at: 
—18°      —15°       —13°         —12° 
44.63      45.26      45.51        45.75%Zn)NO3)2, 


Sp.  gr.  of  Zn(NO3)2+Aq  at  25°. 

0°        +12.5°       18°           25° 
48.66      52.00      53.50      55.90%  Zn(NO3)2, 

36.4°(mpt.)          36°           33.5° 
63.63                   64.73       65.83%  Zn(NO3)2. 

(Funk,  Z.  anorg.  1899,  20.  400.) 

100  g.  Zn(N03)2+Aq  sat.   at  0°  contain 
48.7  g.  Zn(NO3)2;  at  18°,  53.5  g.  Zn(NO3)2. 
(Mylius,  Z.  anorg.  1910,  74.  411.) 
Melts  in  its  crystal  H2O  at  36.4°  (Ordway), 
50°  (Pierre);  boils  at  131°  (Ordway). 
Sp.  gr.  of  solution  sat.  at  18°  =  1.664,  and 
contains    53.9%    Zn(NO3)2.       (Mylius,    B. 
1897,30.1718.) 
Sol.   in  methyl   acetate.      (Naumann,   B. 
1909,  42.  3790);  ethyl  acetate.     (Naumann, 
B.  1910,  43.  314.) 
+9H2O. 
Solubility  in  H20. 
Sat.  solution  contains  at: 
—25°     —22.5°     —20°       —18° 
40.12      40.75      42.03     43.59%  Zn(NO3)2. 
Cryohydrate   is   formed    at   —  29°. 
(Funk,  Z.  anorg.  1899,  20.  401.) 

Concentration  of 
Zn(N03)2+Aq 

Sp.  gr. 

1-normal 

Vr-       " 
Vr-       " 

Vs-       " 

1.0758 
1.0404 
1.0191 
1.0096 

(Wagner,  Z.  phys.  Ch.  1890,  5.  40.) 
Sp.  gr.  of  Zn(NO3)2+Aq.  at  16°. 

Yi  Zn(NO3)2  g.  per  1000 
g.  of  solution 

Sp.  gr.  16°/16° 

0.0000 
0.9950 
2.0061 
4.1535 

8.1824 
17.7760 
34.5920 
68.6780 

1.000000 
1.000814 
1.001646 
1.003413 
1.006733 
1.014702 
1.028890 
1.058644 

(Dijken,  Z.  phys.  Ch.  1897,  24.  108.) 
Sp.  gr.  of  Zn(NO3)2+Aq  at  17.3°,  when  p  = 

r»or    r>emf     atronortVi     rvf    anln+irm  •    r\  —  nVioamrorl 

UTOUO1VJ    y         "      V  WilA-LAO^       \s\J±±\j*        AXi        £^,J.  tl'J.J.J.0       ^SlsJ.        W. 

/Pd          \ 

Zinc  nitrate  ammonia,  Zn(N03)2,  4NH3. 

(ioo=w-) 

Ppt.    (Ephraim,  B.  1915,  48.  638.) 

\               / 

+2/3H20. 

p 

d 

w 

Deliquescent.    Sol.  in  H2O.    (Andre,  C.  R. 

100.  639.) 

47.28 

1.5504 

0.73310 

13ZnO,  3N2O6,  2NH3  +  18H2O. 

41.32 

1.4579 

0.60240 

Insol.   in   cold,    decomp.   by   warm   H20. 

30.86 

1.3136 

0.40535 

(Andre,  C.  R.  1885,  100.  640.) 

29.21 

1.2933 

0.37780 

19.65 
14.39 
11.36 
7.091 

1.1830 
1  .  1284 
1.0988 
1.0597 

0.23246 
0.16232 
0.12478 
0.07515 

Zinc  nitrate  cupric  oxide, 
Zn(NO3)2,    3CuO+3H2O. 
(Mailhe,  A.  ch.  1902,  (7)  27.  169.) 

5.923 

1.0491 

0.06213 

1.574 

1.0118 

0.01593 

Zinc  nitrate  hydrazine,  Zn(NO8)2,  3N2H4. 

1.210 

1.0087 

0.01221 

Decomp.  by  hot  H2O. 

(Barnes,  J.  Phys.  Chem.  1898,  2.  545.) 

Sol.    in    NH4OH.      (Franzen,    Z.    anorg. 
1908,  60.  279.) 

Zirconium  nitrate,  basic,  3ZrO2,  2N2O6. 
Insol.  in  H2O. 

ZrO2,  N2O5.    Easily  sol.  in  H2O  and  alcohol. 
+H2O.    As  above. 

Zirconium  nitrate,  Zr(NO3)4+5H2O  (?). 
Deliquescent,  and  sol.  in  H2O. 

Nitric  oxide,  NO. 
See  Nitrogen  dioxide. 


604 


NITRILOBROMOSMIC  ACID 


Nitrilobromosmic  acid. 


Ammonium  nitri 

[OsNBr5](NH4)2+H20. 

Very  sol.  in  H2O.  Decomp.  in  dil.  aq. 
solution. 

Stable  in  HBr+Aq. 

Insol.  in  organic  solvents.  (Werner,  B. 
1906,  39.  501.) 

Caesium   hydrogen    nitrilopefttabromosmate, 

[OsNBr5]2Cs3H. 
SI.  sol.  in  H2O.    (Werner.) 

Potassium  nitrilotefrabromosmate. 

[OsNBr4]K+2H2O. 

Very  sol.  in  H2O.  Decomp.  in  aq.  solution. 
Stable  in  HBr+Aq.  Insol.  in  organic  sol- 
vents. (Werner.) 

Rubidium  nitrilope^tobromosmate. 

[OsNBr5]Rb2. 

Sol.  in  H2O.  Decomp.  in  dil.  aq.  solution 
after  a  short  time.  (Werner.) 

Nitrilochlorosmic  acid. 

Ammonium  mtrilopen^ochlorosmate. 

(OsNCl6)(NH4)2. 

Sol.  in  H2O;  insol.  in  cone.  HCl+Aq. 
(Werner,  B.  1901,  34.  2702.) 

Cassium  nitriloper^ochlorosmate. 

(OsNCl6)Cs2. 
Sol.  in  H2O.    (Werner.) 

Potassium  nitrilopenZachlorosmate. 
(OsNCl6)K2. 

Sol.  in  H2O;  pptd.  by  HC1;  insol.  in  organic 
solvents.  (Werner.) 

Rubidium  nitrilope^achlorosmate. 

(OsNCl6)Rb2. 

Sol.  in  H2O;  decomp.  in  dil.  neutral  solu- 
tion. (Werner.) 

Nitrilofrimetaphosphoric  acid.  H2NP3O7  = 
PO  .OH 


PO<OH. 

Known  only  in  solution.  (Mente,  A.  248. 
260.) 

Aluminum  nitriloZnwetaphosphate. 

Insol.  in  H2O,  cone.  HC1,  or  HNO3+Aq. 
Slowly  sol.  in  boiling  cone.  H2SO4.  Sol.  in 
warm  NaOH+Aq  or  Na2CO3+Aq  without 
decomp.  Insol.  in  NH4OH+Aq.  (Mente.) 

Barium  -  ,  BaNP3O7. 

Insol.  in  dil.  or  cone,  acids.  Decomp.  by 
boiling  NaOH  or  Na2CO3+Aq.  Insol.  in 
NH4OH+Aq.  (Mente.) 


Cadmium  nitrilofriwetaphosphate. 

Easily  sol.  in  NH4OH+Aq,  or  boiling 
(NH4)2CO3,  or  NaOH+Aq.  (Mente.) 

Calcium ,  CaNP3O7+H2O. 

Sol.  in  cone.  HCl+Aq  by  long  boiling,  and 
more  easily  in  fuming  HNO3+Aq.  Insol.  in 
NH4OH  or  NaOH+Aq.  (Mente.) 

Chromium . 

Slowly  sol.  in  dil.  acids.  Easily  sol.  in 
ammonia.  Sol.  in  cold  NaOH +Aq.  (Mente.) 

Cobalt ,  CoNP3O7+H2O. 

Insol.  in  H2O.  SI.  sol.  in  dil.  acids.  Easily 
sol.  in  NH4OH+Aq.  Decomp.  by  NaOH  or 
Na2CO3+Aq.  (Mente.) 

Copper -. 

Sol.  in  NH4OH+Aq.  Decomp.  by  NaOH 
+Aq.  (Mente.) 

Ferric  — ,  Fe2(NP3O7)3. 

Insol.  in  cone,  acids.  Easily  sol.  in  NH4OH 
+Aq  or  (NH4)2CO3+Aq.  Decomp.  by 
NaOH  or  Na2CO3+Aq.  (Mente.) 

Lead  — . 

Insol.  in  dil.  acids.  Sol.  in  fuming  HNO3. 
Insol.  in  NH4OH+Aq.  Sol.  in  NaOH+Aq. 
(Mente.) 

Magnesium  — ,  MgNP3O7+H2O. 

Slowly  sol.  in  HCl+Aq.  Sol.  in  H2SO4  or 
fuming  HNO3  with  addition  of  Br2.  Insol. 
inNH4OHor(NH4)2CO3+Aq.  (Mente.) 

Manganous  — ,  MnNP307+H2O. 

Insol.  in  dil.  acids.  Very  si.  sol.  in  NaOH+ 
Aq.  Insol.  in  Na2CO3  or  (NH4)2CO3+Aq. 
Easily  sol.  in  NH4OH+Aq.  (Mente.) 

Mercurous ,  Hg2NP3O7. 

Insol.  in  dil.  acids,  NH4OH,  NaOH,  or 
(NH4)2CO3+Aq.  Easily  sol.  in  fuming 
HN03.  (Mente.) 

Nickel -,  NiNP3O7+H2O. 

Insol.  in  dil.  acids,  NH4OH,  or  (NH4)2CO3 
+Aq.  (Mente.) 

Zinc  — ,  ZnNP3O7+2H2O. 

Easily  sol.  in  NH4OH,  NaOH,  or 
(NH4)2C03+Aq.  (Mente.) 

Nitrilosulphonic  acid,  N(SO3H)3. 

Not  known  in  free  state.  (Raschig,  A.  241. 
161.) 

Potassium  nitrilosulphonate,  N(SO3K)3  + 

2H2O. 

Soluble  in  H2O.    (Raschig,  A.  241.  161.) 
Is  identical  with  "potassium  ammoninsul- 

phonate"  of  Claus. 


NITROGEN 


605 


Insol.  in  cold  H2O  (Glaus);  sol.  in  50  pts. 
H2O  at  23°  (Fremy);  in  H2O  at  scarcely  40° 
without  change.  Decomp.  by  boiling.  (Glaus.) 

Potassium  sodium  nitrilosulphonate, 

N(SO,K),(SO,Na). 

Nearly  insol.  in  cold  H2O.  (Raschig,  A. 
241.  161.) 

Sodium  nitrilosulphonate,  N(SO3Na)3. 

Not  isolated  on  account  of  its  extreme 
solubility  in  H2O.  (Raschig,  A.  241.  161.) 

Nitrilocto'sulphophosphoric  acid, 

NP(SH)2. 

Decomp.  by  H2O.  (Stock,  B.  1906,  39. 
2001.) 

Ammonium  mtrilocfasulphophosphate, 

NP(SNH4)2. 

Easily  sol.  in  H2O.  Not  decomp.  by  boiling 
with  alkali.  Decomp.  by  acid.  (Stock.) 

Easily  sol.  in  liquid  NH3.  (Stock,  B.  1903, 
36.  315.) 

Ammomum    hydrogen    nitrilotfisulphophos- 

phate,  SHP(SNH4)N. 
Not  decomp.  by  boiling  with  alkali.     De- 
comp. by  acids.    (Stock,  B.  1906,  39.  1999.) 

Barium  nitrilodisulphophosphate,  BaNPS2  + 

H20. 

Sol.  in  H2O  with  decomp.  Decomp.  by 
hot  H2O.  Not  decomp.  by  warming  with 
alkali.  Decomp.  by  acid.  (Stock.) 

Lead  nitrilocfa'sulphophosphate,  NPS2Pb. 

Sol.  in  liquid  NH3.  Solution  decomp. 
rapidly  with  separation  of  PbS.  (Stock.) 

Sodium  nitriloc&sulphophosphate,  NPSNa2. 

Not  decomp.  by  boiling  with  alkali.  De- 
comp. by  acid.  (Stock.) 

Nitrilosulphuric  acid. 

Ammonium    nitrilosulphate,    N(SO3NH4)3  + 

2H2O. 

Rather  si.  sol.  in  H2O,  but  much  more  sol. 
than  K  salt.  (Divers  and  Haga,  Chem.  Soc. 
1901,  79.  1094.) 

Sodium  nitrilosulphate,  N(SO3Na)3+5H2O. 

Very  sol.  in  H2O.  (Divers  and  Haga, 
Chem.  Soc.  1901,  79.  1097.) 

Nitrilosulphurous  acid. 

Ammomum  nitrilosulphite,  NH(SO2NH4)2. 

Somewhat  deliquescent.  Very  sol.  in  H2O. 
Slowly  decomp.  in  solution.  Decomp.  by 
boiling  with  HC1.  (Divers,  Proc.  Chem.  Soc. 
1901,  17.  163.) 


Nitritocobaltic  chloride. 

Sol.  in  200  pts.  cold  H'2O. 
anorg.  6.  172.) 


(Jorgensen,  Z. 


Nitritoplatincfo'amine  nitrate, 

(N02)2Pt(N2H6N03)2. 
Sol.  in  cold  H2O  with  decomp.;  violently 
decomp.  on  warming.     (Hadow,  Chem.  Soc. 
(2)  4.  345.) 


Nitritopurpureocobaltic  comps. 
See  Xanthocobaltic  comps. 

Nitritopurpureorhodium  comps. 

See  Xanthorhodium  comps. 

Nitrocarbamic  acid. 

Potassium  mtrocarbamate,  NO2.NK.  COOK. 
Decomp.  by  H2O.     (Thiele,  B.  1894,  27. 
1909.) 

Nitro  cobalt,  Co2NO2. 

Decomp.  by  H2O.  (Sabatier  and  Sender- 
ens,  C.  R.  115.  236.) 

Nitro  copper,  CuNO2. 

Violently  decomp.  by  H2O.  (Sabatier  and 
Senderens,  C.  R.  116.  756.) 

Nitroferricyanhydric  acid. 
See  Nitroprussic  acid. 

Nitrogen,  N2. 

Nearly  insol.  in  all  known  solvents. 

1  vol.  recently  boiled  HzO  absorbs  0.0147  vol.  N  at 
15.5°.  (Henry,  1803.) 

1  vol.  recently  boiled  H2O  absorbs  0.025  vol.  N. 
(Dalton.) 

1  vol.  recently  boiled  H2O  absorbs  0.0156  vol.  N  at 
ord.  temp.  (Dalton.) 

1  vol.  H2O  at  t°  and  760  mm.  absorbs  V  vols. 
N  gas  reduced  to  0°  and  760  mm. 


t° 

v 

t 

V 

t° 

V 

0 

0.02035 

7 

0.01713 

14 

0.01500 

1 

0.01981 

8 

0.01675 

15 

0.01478 

2 

0.01932 

9 

0.01640 

16 

0.01458 

3 

0.01884 

10 

0.01607 

17 

0.01441 

4 

0.01838 

11 

0.01577 

18 

0.01426 

5 

0.01794 

12 

0.01549 

19 

0.01413 

6 

0.01752 

13 

0.01523 

20 

0.01403 

(Bunsen.) 

Coefficient     of     absorption    =   0.020346- 
0.00053887t +0.00001 1156t2.     (Bunsen.) 


606 


NITROGEN 


1 1.  H2O  absorbs  ccm.  N  from  atmospheric  air 
at  760  mm.  pressure  and  t°. 


0 

5 

10 


ccm.  N 


19.29 
17.09 
15.36 


15 
20 
25 


ccm.  N 


13.95 
12.80 
11.81 


(Dittmar,  Challenger  Exped.  Report,  vol.  i.) 


0 

5 

10 


ccm.  N 


19.14 
16.93 
15.14 


15 
20 
25 


ccm.  N 


13.73 
12.63 
11.80 


(Hamberg,  1885.) 

Absorption  of  N  by  H2O  at  t°  and  760  mm 
)8  =  coefficient  of  absorption. 


t° 

ft 

t° 

ft 

t° 

ft 

0 

0.02388 

18 

0.01696 

36 

0.01252 

1 

2337 

19 

1667 

37 

1233 

2 

2288 

20 

1639 

38 

1215 

3 

2241 

21 

1611 

39 

1198 

4 

2196 

22 

1584 

40 

1182 

5 

2153 

23 

1557 

41 

1166 

6 

2111 

24 

1530 

42 

1151 

7 

2070 

25 

1504 

43 

1137 

8 

2031 

26 

1478 

44 

1124 

9 

1993 

27 

1453 

45 

1111 

10 

1956 

28 

1428 

46 

1099 

11 

1920 

29 

1404 

47 

1088 

12 

1885 

30 

1380 

48 

1078 

13 

1851 

31 

1357 

49 

1069 

14 

1818 

32 

1334 

50 

1061 

15 

1786 

33 

1312 

60 

1000 

16 

1755 

34 

1291 

100 

1000 

17 

1725 

35 

1271 

(Bohr  and  Bock,  W.  Ann.  44.  318.) 

Absorption  of  N  by  H2O  at  t°  and  760  mm 
ft  =  coefficient  of  absorption;  fti  =  " Solu- 
bility" (see  under  Oxygen). 


t° 

ft 

ft 

0 

0.02348 

0.02334 

1 

2291 

2276 

2 

2236 

2220 

3 

2182 

2166 

4 

2130 

2113 

5 

2081 

2063 

6 

2032 

2013 

7 

1986 

"1966 

8 

1941 

1920 

9 

1898 

1877 

10 

1857 

1834 

11 

1819 

1795 

12 

1782 

1758 

13 

1747 

1722 

14 

1714 

1687 

Absorption  of  N  by  H2O  at  t°. — Continued. 


•  ^° 

ft 

ft 

15 

0.1682 

0.1654 

16 

1651 

1622 

17 

1622 

1591 

18 

1594 

1562 

19 

1567 

1534 

20 

1542 

1507 

21 

1519 

1482 

22 

1496 

1457 

23 

1473 

1433 

24 

1452 

1410 

25 

1432 

1387 

26 

1411 

1365 

27 

1392 

1344 

28 

1374 

1323 

29 

1356 

1303 

30 

1340 

1284 

31 

1321 

1263 

32 

1304 

1243 

33 

1287 

1224 

34 

1270 

1204 

35 

1254 

1185 

36 

1239 

1167 

37 

1224 

1149 

38 

1210 

1131 

39 

1196 

1114 

40 

1183 

1097 

41 

1171 

1082 

42 

1160 

1067 

43 

1149 

1052 

44 

1139 

1037 

45 

1129 

1023 

46 

1120 

1009 

47 

1111 

0995 

48 

1102 

0982 

49 

1094 

0968 

50 

1087 

0955 

52 

1072 

0929 

54 

1058 

0902 

56 

1045 

0876 

58 

1033 

0849 

60 

1022 

0822 

62 

1011 

0794 

64 

1001 

0765 

66 

0992 

0736 

68 

0983 

0707 

70 

0976 

0676 

72 

0970 

0645 

74 

0965 

0614 

76 

0961 

0581 

78 

0959 

0546 

80 

0957 

0510 

82 

0956 

0472 

84 

0955 

0432 

86 

0954 

0388 

88 

0953 

0343 

90 

0952 

0294 

92 

0951 

0242 

94 

0950 

0187 

96 

0949 

0128 

98 

0948 

0086 

100 

0947 

0000 

(Winkler,  B.  24.  3606.) 


NITROGEN 


607 


Coefficient  of  absorption  for  H2O  =0  01432 
at   25°;   0.01621    at   20°;    0.01789    at    15°: 
0.02003  at  10°;  0.02173  at  5°.     (Braun,  Z 
phys.  Ch.  1900,  33.  730.) 

Solubility  in  H2O  at  various  pressures. 

V=  volume  of  the  absorbing  liquid. 
P  =  Hg-pressure  in  metres. 
X  =  coefficient  of  solubility. 

Absorption  of  N2  by  distilled  H2O  at  t°. 
a  =  ccm.  of  N2  absorbed  by  1  1.  of  H2O  at 
t°  and  760  mm. 

t 

a 

t° 

a 

t 

a 

0 
1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 

23.00 
22.50 
22.02 
21.55 
21.09 
20.64 
20.20 
19.77 
19.35 
18.94 
18.54 
18.16 
17.80 
17.46 
17.14 
16.84 
16.56 

17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 

16.29 
16.03 
15.78 
15.54 
15.29 
15.06 
14.84 
14.63 
14.43 
14.23 
14.04 
13.87 
13.71 
13.55 
13.39 
13.23 
13.08 

34 
35 
36 
37 
38 
39 
40 
41 
42 
43 
44 
45 
46 
47 
48 
49 
50 

12.93 
12.79 
12.65 
12.52 
12.39 
12.27 
12.15 
12.04 
11.92 
11.80 
11.68 
11.57 
11.46 
11.35 
11.24 
11.13 
11.02 

V 

t° 

p 

X 

33.  134  com. 

19.4 

0.8910 
1.0453 
1.2488 
1.4764 
1.8111 
2.3961 
2.9074 
3.3411 
4.1382 
4.5958 
5.1103 
5.8349 
6.2767 
7.1059 
7.5815 
8.1074 

0.01617 
0.01616 
0.01611 
0.01608 
0.01602 
0.01597 
0.01585 
0.01579 
0.01561 
0.01554 
0.01546 
0.01528 
0.01515 
0.01499 
0.01487 
0.01473 

(Fox,  Trans.  Faraday  Soc.  1909,  5.  73.) 

Solubility  in  H2O  at  25°  =  0.  1561  .    (Drucker 
and  Moles,  Z.  phys.  Ch.  1910,  75.  418.) 
Solubility  of  N2  in  H2O  at  25°  =0.0231. 
(Calculated  according  to  special  formula,  for 
which  see   original   article.)      (Findlay   and 
Creighton,  Chem.  Soc.  1911,  99.  1315.) 
Coefficient  of  absorption  for  H2O=  0.01689 
at  15°;  0.01670  at  16.2°;  0.01622  at  17.2°. 
(Muller,  Z.  phys.  Ch.  1912,  81.  493.) 

1  1.  sea  water  (sp.  gr.  1.027)  absorbs  com.  N 
from   atmosphere  at   t°   and   760  mm. 
pressure  — 

32.152ccm. 

24.9 

0.8977 
1.0129 
1.1887 
1.5573 
1  .  9846 
2.5171 
2.8781 
3.2956 
4.0947 
4.5581 
5.0529 
5.5935 
6.1956 
7.0333 
7.5596 
?4  .  1846 

0.01498 
0.01493 
0.01491 
0.01487 
0.01482 
0.01478 
0.01463 
0.01455 
0.01440 
0.01434 
0.01426 
0.01413 
0.01408 
0.01382 
0.01377 
0.01369 

t° 

According  to 
Tornoe 

According  to 
Dittmar 

According  to 
Hamberg 

0 
5 
10 
15 
20 
25 

14.40 
13.25 
12.10 
10.95 

15.60 
13.86 
12.47 
11.34 
10.41 
9.62 

14.85 
13.32 
12.06 
11.04 
10.25 
9.62 

(Cassuto,  Phys.  Zeit.  1904,  6.  236.) 

Coefficient  of  absorption  for  H2O  =0.01565 
at  20.18°.  (Hiifner,  Z.  phys.  Ch.  1907,  57. 
615.) 


No.  of  ccm.  of  N2  (containing  1.185%  argon) 
absorbed  by  a  1.  of  sea- water  from  a  free 
dry  atmosphere  of  760  mm.  pressure  at 
given  temperatures. 


Cl 
per  1000 

0* 

4° 

17.02 
16.27 
15.51 
14.75 
14.00 
13.24 

8° 

12° 

16° 

20° 

24° 

28° 

0 
4 
8 
12 
16 
20 

18.64 
17.77 
16.90 
16.03 
15.18 
14.31 

15.63 
14.98 
14.32 
13.66 

13.  on 

12.34 

14.45 
13.88 
13.30 
12.72 
12.15 
11.57 

13.45 
12.94 
12.44 
11.93 
11.73 
10.92 

12.59 
12.15 
11.70 
11.25 
10.81 
10.36 

11.86 
11.46 
11.07 
10.67 
10.27 
9.87 

11.25 
10.89 
10.52 
10.16 
9.80 
9.44 

(Fox,  Trans.  Faraday  Soc.  1909,  5.  77.) 

NITROGEN 


Absorption  of  N2  by  H2SO4+Aq  at  t°. 

1  vol.  alcohol  at  t°  and  760  mm.  dissolves  V 

a  =  coefficient  of  absorption. 

vols.  N  gas  reduced  to  0°  and  760  mm. 

t° 

V 

t° 

V 

Normality  of  the  acid 

t° 

a 

o 

0.12634 

13 

0.  12192 

0 

20.9 

0.0156 

1 

Q!  12593 

14 

0^12166 

4.9 

20.9 

0.0091 

2 

0.12553 

15 

0.12142 

8.9 

20.9 

0.0072 

3 

0.12514 

16 

0.12119 

10.7 

21.2 

0.0066 

4 

0.12476 

17 

0.12097 

20.3 

21.1 

0.0049 

5 

0.12440 

18 

0.12076 

24.8 

21.5 

0.0048 

6 

0.12405 

19 

0.12056 

29.6 

20.8 

0.0051 

7 

0.12371 

20 

0.12030 

34.3 

20.9 

0.0100 

8 

0.12338 

21 

0.12021 

35.8 

21.1 

0.0129 

9 

0.12306 

22 

0.12005 

10 

0  12276 

23 

0.  11990 

(Bohr,  Z.  phys.  Ch.  1910,  71.  49.) 

11 
12 

o!  12247 
0.12219 

24 

o!  11976 

Absorption  of  N2  by  BaCl2+Aq. 
at0  =  coefficient  of  absorption  at  t°. 


(Bunsen's  Gasometry.) 

1  vol.  alcohol  absorbs  0.126338-0.000418t+ 
0.0000060t2  vols.  N  gas.    (Carius,  A.  94. 136.) 


Per  cent  of 
BaCh  in 

a25° 

a20° 

al5° 

alO° 

a5° 

Solubility  in  alcohol  at  25°. 

the  solution 

Vol.  H20 

Vol.  %  alcohol 

Solubility 

13.830 

0.00783 

0.00923 

0.01036 

0.01166 

0.01270 

11.927 

0.00855 

0.00976 

0.01139 

0.01249 

0.01368 

100 

0 

0.01634 

6.903 
6.738 
3.870 

0.01044 
0.01036 
0.01137 

0.01184 
0.01182 
0.01323 

0.01317 
0.01340 
0.01480 

0.01474 
0.01494 
0.01660 

0.01598 
0.01628 
0.01802 

80 
67 

20 
33 

0.01536 
0.01719 

3.325 

0.01190 

0.01346 

0.01502 

0.01681 

0.01826 

0 

100 

0.1432 

(Braun,  Z.  phys.  Ch.  1900,  33.  733.) 

Absorption  of  N2  by  NaCl+Aq. 
ot°  =  coefficient  of  absorption  at  t°. 


(Just,  Z.  phys.  Ch.  1901,  37.  361.) 

1  vol.  ether  absorbs  0.15  vol.  N  (Dobereiner) ;  1  vol. 
caoutchine  absorbs  5  vols.  N  in  5  weeks  (Himly). 

Solubility  of  N2  in  ether  =  0.2580  at  0°; 
0.2561  at  10°.  (Christoff,  Z.  phys.  Ch.  1912, 
79.  459.) 


Per  cent  of 
NaCl  in 
the  solution 

a25° 

a20° 

al5° 

alO° 

ao° 

Solubility  in  organic  solvents 

Solvent 

Solubility 
at  25°  C. 

Solu- 
bility 
at20°C. 

ds 
dt 

11.732 
10.945 
8.135 
8.033 
6.595 
6.400 
4.196 
3.880 
2.120 
2.100 
0.686 
0.671 

0.00470 
0.00565 
0.00749 
0.00729 
0.00802 
0  .  00826 
0.00990 
0.01005 
0.01131 
0.01133 
0.01295 
0.01304 

0.00657 
0.00703 
0.00872 
0.00871 
0.00972 
0  .  00975 
0.01151 
0.01168 
0.01311 
0.01314 
0.01477 
0.01484 

0.00810 
0.00824 
0.01014 
0.00995 
0.01120 
0.01134 
0.01294 
0.01316 
0.01469 
0.01467 
0.01640 
0.01642 

0.00930 
0.00912 
0.01131 
0.01121 
0.01252 
0.01259 
0.01451 
0.01475 
0.01638 
0.01656 
0.01833 
0.01845 

0.01016 
0.01052 
0.01266 
0.01248 
0.01380 
0.01375 
0.01579 
0.01615 
0.01795 
0.01805 
0.01994 
0.02000 

Glycerine 

Water 
Aniline 
Carbon  bisulphide 
Nitrobenzene 
Benzene 
Glacial  acetic  acid 
Xylene 
Amyl  alcohol 
Toluene 
Chloroform 
Methyl  alcohol 
Ethyl  alcohol  (99.8%) 
Acetone 
Amyl  acetate 
Ethyl  acetate 
Isobutyl  aceate 

Not 
measurable 
0.01634 
0.03074 
0.05860 
0.06255 
0.1159 
0.1190 
0.1217 
0.1225 
0.1235 
0.1348 
0.1415 
0.1432 
0.1460 
0.1542 
0.1727 
0.1734 

0  .  01705 
0.02992 
0  .  05290 
0.06082 
0.114 
0.1172 
0.1185 
0.1208 

0:1186 

0.1282 
0.1348 
0.1400 
0.1383 
0.1512 
0.1678 
0.1701 

—0.000142 
+0.000164 
+0.00114 
+0.000346 
+0.0009 
+0.00036 
+0  .  00062 
+0.00034 
+0  .  00098 
+0.00132 
+0  .  00134 
+0.00064 
+0.00154 
+0.0006 
+0  .  00098 
+0.00066 

(Braun,  I  c.) 

• 
At  —191.5°  liquid  oxygen  dissolves  458 

t.iTYiAH  ifs  vr»l     rvr  RC\  7  r»«vr  r>onf  r»f  i+a  ixroinrlit  nf 

gaseous  nitrogen.     (Erdmann,  B.  1904,  37. 
1191.) 


At  18°  and  760  mm.  100  vols.  H2O  or  alcohol  of  0.84 
sp.  gr.  absorb  4.2  vols.  N  gas.      (de  Saussure,  1814.) 


(Just,  Z.  phys.  Ch.  1901,  37.  361.) 

Coefficient  of  absorption  for  petroleum  = 
0.117  at  20°;  0.135,  at  10°.  (Gniewasz  and 
Walfisz,  Z.  phys.  Ch.  1.  70.) 


NITROGEN 


609 


Absorption  of  N2  by  propionic  acid+Aq. 
at0  =  coefficient  of  absorption  at  t°. 

Absorption  of  N2  by  organic  substances  +Aq 
at  15°. 

P  =  %  of  the  organic  substance  in  the  sol- 
vent. 
/315°  =  coefficient  of  absorption  at  15°. 
S15°  =  Solubility  at  15°, 

Per  cent  of 
propionic 
acid  in  the 
solution 

<*25° 

a20° 

al5° 

•alO° 

a5° 

11.220 
11.023 
9.537 
9.155 
6.066 
5.891 
4.081 
3.816 

0.01301 
0.01295 
0.01336 
0.01329 
0.01335 
0.01338 
0.01365 
0.01371 

0.01463 
0.01447 
0.01471 
0.01469 
0.01476 
0.01480 
0.01541 
0.01547 

0.01593 
0.01585 
0.01634 
0.01630 
0.01637 
0.01648 
0.01688 
0.01674 

0.01779 
0.01800 
0.01823 
0.01845 
0.01855 
0.01872 
0.01919 
0.01915 

0.01951 
0.01977 
0.02040 
0.02026 
0.02077 
0.02089 
0.02095 
0.02087 

Organic  substance 
used 

p 

M| 

S15° 

Chloralhydrate 

0 
0 
0 
6.9 
14.0 
15.0 
23.6 
26.1 
37.6 
48.9 
49.3 
61.3 
70.9 
71.2 
78.3 
79.1 

0.01725 
0.01675 
0.01706 
0.0164 
0.0154 
0.0152 
0.0134 
0.0141 
0.0123 
0.0115 
0.0118 
0.0114 
0.0131 
0.0130 
0.0152 
0.0156 

O.oi796 

O.oi73 
0.0162 
0.0160 
0.0141 
0.0149 
0.0130 
0.0121 
0.0124 
0.0120 
0.0138 
0.0137 
0.0160 
0.0165 

(Braun,  Z.  phys.  Ch.  1900,  33.  732.) 

Solubility  of  N2  in  isobutyric  acid+Aq  at  t°. 

P  =  Corrected  pressure  at  end  of  experi- 
ment in  mm.  Hg  at  0°. 
S  =  Solubility  of  N2. 

Solvent 

t 

P 

8 

Pure  isobutyric 
acid 

25.05 

262.6 
388.3 
566.1 
662.4 
783.5 
832.2 

0.1609(?) 
0.1640 
0.1647 
0.1656 
0.1656 
0.1656 

Glycerine 

0 
0 
15.7 
15.7 
29.9 
46.6 
57.6 
67.1 
72.8 
74.7 
77.0 
85.1 
87.3 
88.5 
99.25 

0.01707 
0.01708 
0.01425 
0.01376 
0.01087 
0.00840 
0.00698 
0.00635 
0.00552 
0.00597 
0.00527 
0.00482 
0.00492 
0.00536 
0.00524 

37.5%  solution 
of  isobutyric 
acid+Aq 
Vapor  pressure  = 
21.6  mm. 

23.02 

246 
492 
563 
836 

867 

2 

2 
6 

3 
3 

0.0393 
0.0393 
0.0393 
0.0400 
0.0401 

it 

Vapor  pressure  = 
30.6  mm. 

29.02 

231 
468.4 
480.7 
536 
656 
720 

0.0373 
0.0384 
0.0383 
0.0385 
0.0384 
0.0386 

(Drucker  and  Moles,  Z.  phys.  Ch.  1910,  76. 

434.) 

Absorption  of  N2  by  chloralhydrate+Aq. 

t°  =  temp.  of  the  solution. 
P  =  %  chloralhydrate  in  the  solution. 
/3t°  =  coefficient  of  absorption  at  t°. 
01 5°  =  coefficient  of  absorption  at  15°. 


(Hammel,  Z.  phys.  Ch.  1915,  90.  121.) 


Absorption  of  N2  by  glycerine +Aq. 

t°  =  temp.  of  the  solution. 
P  =  %  glycerine  in  the  solution. 
/3t°  =  coefficient  of  absorption  at  t°: 
015°  =  coefficient  of  absorption  at  15°. 


t° 

P 

/3t° 

/3i5° 

15.6 
15.4 
16.4 
16.9 
17.0 
15.3 
14.8 

15.8 
28.2 
37.25 
47.0 
56.52 
71.5 
78.8 

0.01574 
0.01418 
0.01288 
0.01260 
0.01230 
0.01415 
0.01447 

0.01580 
0.01422 
0.01300 
0.01275 
0.01245 
0.01420 
0.01495 

(Miiller,  Z.  phys.  Ch.  1912,  81.  499.) 


t° 

p 

&> 

015° 

16.1 

25.0 

0.01240 

0.01266 

15.6 

42.2 

0.00966 

0.00976 

14.7 

51.5 

0.00759 

0.00759 

14.9 

58.0 

0.00703 

0.00703 

15.9 

80.25 

0.00520 

0.00530 

16.2 

90.0 

0.00570 

0.00583 

18.0 

95.0 

0.00578 

0.00716 

(Miiller,  Z.  phys.  Ch.  1912,  81.  496.) 

610 


NITROGEN  BROMOPHOSPHIDE 


Solubility  of  N2  in  glycerine +Aq  at  25°. 
G=  %  by  wt.  of  glycerine  in  the  solvent. 
S= solubility  of  N2. 

P  =  corrected  pressure  at  end  of  experiment 
in  mm.  Hg  at  0°. 


G 

p 

s 

16 

598.4 

0.0103 

a 

915.5 

0.0103 

29.7 

556.5 

0.0067 

a 

846.5 

0.0068 

48.9 

617.7 

0.0052 

n 

859.8 

0.0051 

74.5 

588.5 

0:0025 

84.1 

637.3 

0.0024 

tt 

757.0 

0.0024 

(Drucker  and  Moles,  Z.  phys.  Ch.  1910,  76. 
418.) 

Absorption  of  N2  by  sucrose +Aq. 
t°=temp.  of  the  solution. 
P  =  %  sucrose  in  the  solution. 
/3t°  =  coefficient  of  absorption  at  t°. 
/315°  =  coefficient  of  absorption  at  15°. 


t° 

p 

/3t° 

015° 

16.2 
17.2 

0.01670 
0.01622 

0.01700 
0.01688 

16.8 
16.9 
17 
17.8 
18 
17.7 

11.38 
20.00 
29.93 
30.12 
47.89 
48.57 

0.01432 
0.01233 
0.01025 
0.01033 
0.00742 
0.00658 

0.01480 
0.01280 
0.01053 
0.01090 
O.OQ785 
0.00700 

(Miiller,  Z.  phys.  Ch.  1912,  81.  493.) 

Absorption  of  N2  by  organic  substances +Aq 
att°. 

V  =  absorbed  volume  reduced  to  0°  and 
760  mm. 

a  =  coefficient  of  absorption. 


Solution 

Vol.  of 
solution 
com. 

t° 

V 

com. 

a 

N-dextrose 

409.94 

20.18 

4.55 

0.01215 

^N-dextrose 

409.94 

20.21 

5.14 

0.01380 

^N-dextrose 

409.94 

20.2 

5.51 

0.01480 

N-levulose 

409.94 

20.25 

4.27 

0.01221 

N-arabinose 

409.94 

20.21 

4.40 

0.01203 

jN-erythritol 

409.94 

20.25 

4.87 

0.01321 

:N-alanine 

409.94 

20.19 

4.445 

0.01213 

N-glycocoll 

409.94 

20.16 

4.47 

0.01212 

N-urea 

409.94 

20.18 

5.37 

0.01477 

N—  acetamide 

409.94 

20.22 

5.385 

0.01475 

(Hiifner,  Z.  phys.  Ch.  1907,  67.  618-621.) 

.Nitrogen  bromide,  NBr3. 
Decomp.  under  H2O. 


Nitrogen  bromophosphide,  PBr2N. 

Insol.  in  H2O.  Sol.  in  ether,  less  sol.  in  CS2 
or  CHC13.  (Besson,  C.  R.  114.  1479.) 

Nitrogen  bromosulphide. 
See  Nitrogen  sulphobromide. 

Nitrogen  chloride,  NC13. 

Very  unstable.  Explodes  when  heated  to 
93°  or  by  contact  with  other  substances. 
Insol.  in  H2O,  but  is  decomp.  thereby  (in  24 
hours  by  cold  H2O).  Sol.  in  CS2,  PC13,  and 
S2C12.  (H.  Davy,  Phil.  Trans.  1813,  1.  242.) 

Sol.  in  C6H6,  CS2,  CHC16,  CC14.  (Hentschel 
B.  1897,  30.  1434.) 

Nitrogen  chlorophosphide,  N3P3C16. 

Insol.  in  H2O,  but  slowly  decomp.  thereby. 
Insol.  in  hot  H2SO4,  HC1,  or  HNO3+Aq. 
Decomp.  by  hot  fuming  HNO3.  Sol.  in  al- 
cohol; very  sol.  in  ether,  but  these  solutions 
gradually  decompose.  Sol.'  in  CS2,  CHC13, 
C6H6,  and  oil  of  turpentine. 

Sol.  in  POC13.  (Gladstone,  Chem.  Soc.  3. 
138.) 

Nitrogen  chlorosulphide. 
See  Nitrogen  sulphochloride. 

Nitrogen  fluoride. 
Very  explosive.    (Warren,  C.  N.  56.  289.) 

Nitrogen  worioiodamine,  NH2I. 

Very  rapidly  decomp.  by  H2O  into  N2H3I3. 
(Raschig,  A.  230.  212.) 

Nitrogen  diiodamine,  NHI2. 

Properties  as  triioddiamiue. 

Nitrogen  Zniodcftamine,  NH3,  NI3. 

Decomp.  by  H2O.    (Raschig,  A.  230.  212.) 
Insol.  in  absolute  alcohol.     Sol.  with  de- 
comp. in  HCl+Aq.    (Bunsen.) 

Nitrogen  iodide,  N3I. 
See  Tn'azoiodide. 

Nitrogen  iodide,  NI3. 

Insol.  in  H2O,  but  slowly  decomp.  thereby. 
Sol.  in  HCl+Aq.  Sol.  in  KCN+Aq.  (Mil- 
Ion,  J.  pr.  17.  1.) 

Sol.  in  Na2S203+Aq.  (Guyard,  C.  R.  97. 
526.) 

Sol.  in  KSCN+Aq.    (Raschig,  A.  230. 212.) 

Nitrogen  iodide  ammonia,  NI3,  3NH3;  NIa, 
2NH3;  and  NI3,  NH3. 

(Hugot,  C.  R.  1900,  130.  507.) 

NI3,  12NH3.  Ppt.;  insol.  in  ether.  (Ruff, 
B.  1900,  33.  3028.) 


NITROGEN  OXIDE 


611 


Nitrogen  monoxide,  N2O. 

(a.)  Liquid.    Miscible  with  alcohol  or  ether. 
(b.)  Gas. 

1  vol.  H2O  absorbs  0.78-0.86  vol.  N2O  at  ordinary 
temp.  (Henry) ;  0.80  vol.  at  ordinary  temp.  (Dalton) ; 
0.76  vol.  at  ordinary  temp,  (de  Saussure) ;  0.708  vol.  at 
18°  (Pleisch);  0.54  vol.  (Davy). 

1  vol.  H2O  at  t°  and  760  mm.  absorbs  V  vols. 
N2O,  reduced  to  0°  and  760  mm. 


t° 

v 

t 

V 

0 

.3052 

13 

0.8304 

1 

.2605 

14 

0.8034 

2 

.2172 

15 

0.7778 

3 

.  1752 

16 

0.7535 

4 

.1346 

17 

0.7306 

5 

.0954 

18 

0.7090 

6 

.0575 

19 

0.6888 

7 

.0210 

20 

0.6700 

8 

0.9858 

21 

0.6525 

9 

0.9520 

22 

0.6364 

10 

0.9196 

23 

0.6216 

11 

0.8885 

24 

0.6082 

12 

0.8588 

(Bunsen's  Gasometry.) 

1  vol.  H20  absorbs  1.30521-0.0453620t  + 
0.00068430t2  vols.  N2O  at  t°  and  760  mm. 
(Bunsen.) 

Coefficient  of  absorption  by  H2O=  0.01883 
at  15°.  (Steiner,  Z.  phys.  Ch.  1895,  18.  14.) 

Coefficient  of  absorption  by  H->O=  0.600 
at  23.5°;  0.773  at  15.5°;  0.951  at  8.1°.  (Gor- 
don, Z.  phys.  Ch.  1895,  18.  4.) 

Absorption  of  N2O  by  H2O  at  t°. 


t 

Coefficient  of  absorption 

25 
20 
15 
10 
5 

0.5752 
0.6654 
0.7896 
0.9479 
1.1403 

(Roth,  Z.  phys.  Ch.  1897,  24.  123.) 

Solubility  in  H2O  at  25° =0.5942;  at  20°  = 
0.6756;  at  15°  =0.7784;  at  10°  =  0.9101;  at 
5°  =  1.067.  (For  formula  for  "solubility," 
see  under  oxygen.)  (Geffcken,  Z.  phys.  Ch. 
1904,  49.  278.) 

Solubility  of  N2O  in  H2O  =0.592  at  25°  and 
758-1362  mm.  pressure.  (Findlay  and 
Creighton,  Chem.  Soc.  1910,  97.  538.) 

100  vols.  H2SO4  (sp.  gr.  =  1.84)  absorb  75.7 
vols.  N2O;  100  vols.  H2SO4+Aq  (sp.  gr.= 
1.80)  absorb  66.0  vols.  N2O;  100  vols.  H2SO4 
+Aq  (sp.  gr.  =  1.705)  absorb  39.1  vols.  N2O; 
100  vols.  H2S04+Aq  (sp.  gr.  =  1.45)  absorb 
41.6  vols.  N2O;  100  vols.  H2SO4+Aq  (sp.  gr. 
=  1.25)  absorb  33.0  vols.  N2O. 

CaCl2+Aq,  and  NaCl+Aq  absorb  con- 
siderable amounts  of  N2O.  (Lunge,  B.  14. 
2188.) 


Absorption  by  acids +Aq. 
M  =  content  in  gram-equivalents  per  liter. 
S  =  solubility  (see  under  Oxygen). 
Absorption  of  N2O  by  HNO3+Aq. 


M 

S25° 

S  15° 

0.610 
0.614 
1.253 
1.254 
2.405 
2.435 

0.5969 
0.5980 
0.6045 
0.6061 
0.6156 
0.6149 

0.7770 
0.7766 
0.7767 
0.7767 
0.7735 
0.7737 

(Geffcken,  Z.  phys.  Ch.  1904,  49.  278.) 
Absorption  of  N2O  by  HCl-fAq. 

M 

S25° 

S  15° 

0.549 
0.550 
1.089 
1.093 
2.300 
2.340 

0.5775 
0.5759 
0.5670 
0.5657 
0.5546 
0.5564 

0.7550 
0.7528 
0.7360 
0.7347 
0.7103 
0.7122 

Absorptic 

(Geffcken.) 
D,,  _,f  TSJ  n  Kir  ^2kO4 

n  oi  IN  2u  oy       2      i~Aq. 

M 

S25° 

S  15° 

0.523 
0.526 
1.050 
1.054 
2.042 
2.047 
2.971 
2.963 
3.897 
3.973 

0.5648 
0.5657 
0.5426 
0.5419 
0.5083 
0.5087 
0.4819 
0.4820 
0.4569 
0.4577 

0.7328 
0.7340 
0.6997 
0.6984 
0.6440 
0.6428 
0.6024 
0.6030 
0.5648 
0.5640 

(Geffcken.) 
Absorption  of  N2O  by  H3P04+Aq  at  t°. 

t° 

5 
10 
15 
20 
25 

%  of  HsPCU 

3.38%        4.72%        8.84% 

9.89%        13.35% 

1.057      1.0365    0.9883 
0.8827    0.8665    0.8296 
0.7388    0.7258    0.6977 
0.6253    0.6147    0.5926 
0.5427    0.5329    0.5143 

0.9635   0.9171 
0.8101    0.7711 
0.6826   0.6505 
0.5810   0.5555 
0.5054    0.4860 

(Roth,  Z.  phys.  Ch.  1897,  24.  134.) 

100  vols.  cone.  FeSO4+Aq  absorb  19.5  vols. 
N2O. 

Solubility  of  N2O  in  a  solution  containing 
47.7  g.  -Fe(OH)3  per  litre  at  25° =0.5799; 
47.9  g.  Fe(OH)8  per  litre  at  25°  =  0.5787. 
(Geffcken,  Z.  phys.  Ch.  1904,  49.  299.) 


612 


NITROGEN  OXIDE 


100  vols.  KOH+A 
18.7  vols.  N2O;  100  v 
pyrogallol  absorb  18 
NaOH+Aq  (sp.  gr.= 
sorb  23.1  vols.  N2O;  1 
with  pyrogallol  absor 

Absorption  of  IS 
M  =  content  in  grai 
S  =  solubility  (see  u 

q  (sp. 
ols.  K( 
1  volj 

gr.  =  1.12)  absorb 
3H+Aq  sat.  with 
3.  N2O;  100  vols. 
(7%  NaOH)  ab- 
3.  NaOH+Aqsat. 
vols.  N2O. 

KOH+Aq. 
valents  per  litre. 
>xygen). 

Absorption  of  N2O  by  salts  +Aq  at  15°. 
M=  number  of  molecules  of  salt  per  litre, 
a  =  coefficient  of  absorption. 

-1.1) 

00  vols 
b28.0 

f20by 
n-eqii] 
nder  c 

Salt 

M 

a 

KC1 

3.554 
2.909 
1.755 
1.051 
0.526 

0.0892 
0.1012 
0.1279 
0.1489 
0.1667 

M 

S  25°                         S  15° 

KNO3 

2.430 
1.820 
1.541 
0.879 
0.482 

0.1180 
0.1311 
0.1391 
0.1559 
0.1683 

0.541 
0.542 
1.074 
1.082 

0.5087                0.6591 
0.5093                0.6595 
0.4252                0.5427 
0.4221               0.5392 

K2CO8 

4.352 
2.939 
2.156 
1.376 
0.690 
0.341 
0.209 

0.0160 
0.0285 
0.0462 
0.0761 
0.1183 
0.1501 
0.1628 

(Geffcken,  Z.  phys.  Ch.  1904,  49.  278.) 

Coefficient  of  solubility  of  N2O  in  salts  +Aq 
at  t°. 

Salt 

Concentration 
of  salt 

Coeff.  of  absorption  at 

G.  per 

100  g. 
solu- 
tion 

G. 
mol. 
per  1. 

5° 

10° 

15° 

20° 

NaCl 

4.815 
2.801 
2.049 
0.825 

0.0595 
0.0925 
0.1130 
0.1548 

CaCl2 

5.79 
9.86 
13.99 

0.547 
0.964 
1.416 

0.819 
0.608 
0.510 

0.697 
0.586 
0.441 

0.591 
0.509 
0.380 

0.500 
0.435 
0.328 

NaNO2 

5.711 
3.980 
2.656 
1.413 
0.679 

0.0578 
0.0810 
0.1052 
0.1370 
0.1603 

LiCl 

1.35 
3.85 

1    4.8 

0.319 
0.928 

2.883 

0.986 
0.878 
0.606 

0.831 
0.743 
0.512 

0.700 
0.629 
0.437 

0.599 
0.536 
0.382 

Na2CO3 

1.218 
0.819 
0.438 
0.207 

0.0839 
0.1082 
0.1385 
0.1639 

Li2SO4 

2.37 
5.46 
8.56 

0.219 
0.521 
0.836 

0.934 
0.795 
0.646 

0.792 
0.665 
0.555 

0.670 
0.557 
0.477 

0.569 
0.474 
0.415 

MgS04 

5.90 
7.66 
10.78 

0.521 
0.687 
0.997 

0.766 
0.708 
0.569 

0.664 
0.586 
0.491 

0.561 

0.486 
0.417 

0.471 
0.414 
0.346 

Na2S04 

1.364 
0.638 
0.335 

0.0775 
0.1254 
0.1519 

KC1 

4.90 
7.64 
14.58 
22.08 

0.676 
1.037 
2.187 
3.414 

0.879 
0.799 
0.654 
0.544 

0.751 
0.693 
0.574 
0.459 

0.643 
0.591 
0.500 
0.390 

0.555 
0.494 
0.430 
0.339 

LiCl 

3.734 
1.800 
0.835 

0.0990 
0.1370 
0.1619 

MgS04 

2.501 
1.631 
0.936 
0.433 

0.0499 
0.0797 
0.1159 
0.1501 

K2S04 

2.62 

4,78 

0.154 
0.285 

0.986 
0.918 

0.831 
0.763 

0.701 
0.637 

0.605 
0.542 

NaCl 

6.20 

8.88 
12.78 

1.107 
1.614 
2.391 

0.800 
0.713 
0.634 

0.682 
0.603 
0.532 

0.585 
0.510 
0.449 

0.509 
0.434 
0.386 

ZnSO4 

2.180 
1.277 
0.899 
0.397 

0.0605 
0.0961 
0.1175 
0.1525 

Na2S04 

5.76 
8.53 
12.44 

0.427 
0.646 
0.974 

0.808 
0.692 
0.559 

0.677 
0.574 
0.486 

0.584 
0.482 
0.417 

0.495 
0.416 
0.354 

CaCl2 

2.962 
2.556 
1.827 
1.122 
0.578 
0.321 

0.0519 
0.0619 
0.0839 
0.1138 
0.1450 
0.1619 

SrCl2 

3.31 
5.73 
13.24 

0.215 
0.380 
0.939 

0.928 
0.848 
0.644 

0.788 
0.709 
0.547 

0.671 
0.610 
0.463 

0.578 
0.556 
0.390 

(Gordon,  Z.  phys.  Ch.  1895,  18.  5.) 

(Steiner,  Z.  phys.  Ch.  1895,  18.  14-5.) 

NITROGEN  OXIDE 


613 


Coefficient  of  absorption  of  N2O  by  NaCl-f- 
Aq  at  t°. 

Absorption  of  N2O  by  salts  +Aq.  — 
Continued. 

t° 

Per  cent 

of  NaCl 

Salt 

M 

S25° 

S  15° 

0.990             1.808 

3.886 

5.865 

KBr 

0.546 
0.550 
0.937 
0.959 

0.5306 
0.5318 
0.4908 
0.4899 

0.6877 
0.6892 
0.6352 
0.6334 

5 
10 
15 
20 
25 

1.0609      1.0032 
0.8812     0.8383 
0.7339     0.7026 
0.6191      0.5962 
t).5363     0.5190 

0.9131 
0.7699 
0.6495 
0.5520 
0.4775 

0.8428 
0.7090 
0.5976 
0.5088 
0.442,4 

•RbCl 

0.439 
0.444 
0.977 
0.993 
0.558 
0.559 
1.070 
1.102 

0.5399 
0.5386 
0.4873 
0.4846 
0.5218 
0.5217 
0.4673 
0.4639 

0.7050 
0.7053 
0.6306 
0.6276 
0.6782 
0.6787 
0.6046 
0.6020 

(Roth,  Z.  phys.  Ch.  1897,  24.  139.) 

Absorption  of  N2O  by  salts  +Aq  at  20°. 
C  =  concentration  of  the  solution  in  terms 
of  normal, 
a  =  coefficient  of  absorption. 
Absorption  of  N2O  by  KNO3+Aq  at  20°. 

(Geffck 

Solubilit 
39.6  g.  As2' 
As2S3  per  h 

1  vol.  alco 
vols.  N2C 

3n,  Z.  phys. 

y  of  N2O  ii 
33  per  litre 

Ch.  1904,  49.  278.) 

i  a  solution  containing 
at  25°  =  0.5819;  42.4  g. 
0.5833.    (Geffcken.) 

id  760  mm.  absorbs  V 
d  to  0°  and  760  mm. 

P 

C 

a 

0 
1.063 
2.720 
5.389 
10.577 

0.1061 
0.2764 
0.5630 
1  .  1683 

0 
0 
0 
0 
0 

6270 
6173 
.6002 
.5713 
.5196 

10!  at  t°  ai 
>  gas  reduce 

t° 

V 

t 

v 

0 
1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 

4.1780 
4.1088 
4.0409 
3.9741 
3.9085 
3.8442 
3.7811 
3.7192 
3.6585 
3.5990 
3.5408 
3.4838 
3.4279 

13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 

3.3734 
3.3200 
3.2678 
3.2169 
3.1672 
3.1187 
3.0714 
3.0253 
2.9805 
2.9368 
2.8944 
2.8532 

Absorption  of  N2O  by  NaNO3+Aq  at  20°. 

P 

C 

a 

0 
1. 
2 

5. 

8. 

124 
531 
077 
701 

0.1336 
0.3052 
0.6286 
1  .  1200 

0 
0 
0 
0 
0 

.6270 
.6089 
.5876 
.5465 
.4926 

(Knopp,  Z.  phys.  Ch. 

1904,  48. 

107.) 

Absorption  of  N2O  by  salts+Aq. 
M  =  content  in  gram-equivalents  per  litre. 
S  =  solubility. 


Salt 

M 

S25° 

S  15° 

NH4C1 

0.598 
0.600 
1.158 
1.166 

0.5532 
0.5504 
0.5223 
0.5200 

0.7203 
0.7185 
0.6800 
0.6775 

KI 

0.550 
0.557 
0.886 
0.913 
0.514 
0.545 

0.5367 
0.5344 
0.5025 
0.5012 
0.5428 
0.5406 

0.6950 
0.6916 
0.6466 
0.6442 
0.7074 
0.7036 

LiCl 

0.558 
0.561 
1.057 
1.059 

0.5276 
0.5278 
0.4760 
0.4773 

0.6884 
0.6877 
0.6163 
0.6146 

(Bunsen's  Gasometry.) 

Coefficient  of  absorption  =  4. 17805- 
0.0698160t+0.0006090t2.  (Carius.) 

At  18°  and  760  mm.,  100  vols.  H2O  absorb  76  vols. 
N2O;  100  vols.  alcohol  of  0.840  sp.  gr.  absorb  153  vols.; 
100  vols.  rectified  naphtha  of  0.784  sp.  gr.  absorb  254 
vols.;  100  vols.  oil  of  lavender  of  0.880  sp.  gr.  absorb 
275  vols.;  100  vols.  olive  oil  of  0.915  so.  gr.  absorb  150 
vols.;  100  vols.  sat.  KCl+Aq  (23%  KC1)  of  1.212  sp. 
gr.  absorb  29  vols.  (de  Saussure,  1814.) 

1  vol.  oil  of  turpentine  absorbs  2.5-2.7  vols.  N2O. 
(de  Saussure.) 

Absorption  of  N2O  by  glycerine +Aq  at  t°. 


t 

%  by  weight  of  glycerine 

3.460% 

6.726% 

12.120% 

16.244% 

25 
20 
15 
10 
5 

0.5558 
0.6468 
0.7672 
0.9172 
1.0967 

0.5415 
0.6303 
0.7454 
0.8871 
1.0552 

0.5268 
0.6050 
0.7098 
0.8411 
0.9990 

0.5083 
0.5851 
0.6857 
0.8102 
0.9586 

(Roth,  Z.  phys.  Ch.  1897,  24.  128.) 


614 


NITROGEN  OXIDE 


Absorption  of  N2O  by  urea+Aq  at  t°. 

Absorption  of  N2O  by  oxalic  acid+Aq  at  t°. 

t° 

%  by  weight  of  urea 

t° 

Coeff.  of  abs.  in  H2C2O4  +Aq  of  given 
%  strength 

3.312% 

4.974% 

6.366% 

7.296% 

9.966% 

8.122% 

3.699% 

25 
20 
15 
10 
5 

0.5686 
0.6533 
0.7708 
0.9209 
1.1040 

0.5669 
0.6558 
0.7732 
0.9201 
1.0964 

0.5588 
0.6539 
0.7605 
0.9086 
1.0880 

0.7502 
0.6553 
0.7722 
0.9208 
1  .  1012 

Q.5689 
0.6508 
0.7614 
0.9007 
1.0685 

25 
20 
15 
10 
5 

0.5786 
0,6694 
0.7940 
0.9526 
1.1450 

0.5643 
0.6538 
0.7745 
0.9264 
1  .  1094 

(Roth,  Z.  phys.  Ch.  1897,  24.  124.) 


Absorption  of  N2O  by  sugar +Aq  at  15°. 


Number  of  molecules 
of  Ci2H22On  per  litre 

Coefficient  of  absorption 

1.699 
0.993 
0.520 

0.0892 
0.1284 
0.1561 

(Steiner,  Z.  phys.  Ch.  1895,  18.  15.) 


Absorption  of  N2O  by  organic  substances + 
Aq. 

C  =  concentration  of  the  solution  in  terms 
of  normal. 

a  =  coefficient  of  absorption. 
Absorption  of  N2O  by  chloral  hydrate +Aq 
at  20°. 


P 

C 

a 

0 
2.947 
6.848 
13.48 
16.15 
19.60 
24.02 

0^184 
0.445 
0.942 
1.165 
1.474 
1.911 

0.6270 
0.6182 
0.6128 
0.5960 
0.5891 
0.5793 
0.5675 

(Knopp,  Z.  phys.  Ch.  1904,  48.  106.) 


Absorption  of  N2O  by  propionic  acid+Aq  at 
20°. 


P 

C 

a 

0 
1.492 
5.702 
13.680 
15.011 
25.589 

0'.2045 
0.816 
2.140 
2.385 
4.645 

0.6270 
0.6323 
0.6369 
0.6504 
0.6534 
0.7219 

(Knopp,  Z.  phys.  Ch.  1904,  48.  107.) 


(Roth,  Z.  phys.  Ch.  1897,  24.  130.) 


Coefficient  of  absorption  for  petroleum  = 
2.11  at  20°;  2.49  at  10°.  (Gniewasz  and 
Walfisz,  Z.  phys.  Ch.  1.  70.) 

The  solubility  of  N2O  in  various  colloidal 
solutions  has  been  determined  by  Findlay 
and  Creighton  (Chem.  Soc.  1910,  97.  538),  for 
which  see  original  article. 


Nitrogen  dioxide,  NO. 

1  vol.  H2O  absorbs  0.1  vol.  NO  gas  at  ordinary  temp. 
(Davy) ;  1  vol.  absorbs  0.05  vol.  (Henry) ;  1  vol.  absorbs 
1/27  vol.  (Dalton.) 

Absorption  of  NO  by  H2O  at  760  mm. 

pressure. 

0  =  Coefficient  of  absorption. 
./3'  =  "  Solubility." 


t° 

ft 

0' 

t° 

]8 

? 

0 

0.07381 

0.07337 

55 

0.03040 

0.02570 

5 

6461 

6406 

60 

2954 

2375 

10 

5709 

5640 

65 

2877 

2169 

15 

5147 

5061 

70 

2810 

1947 

20 

4706 

4599 

75 

2751 

1706 

25 

4323 

4189 

80 

2700 

1439 

30 

4004 

3838 

85 

2665 

1146 

35 

3734 

3529 

90 

2648 

0817 

40 

3507 

3254 

95 

2638 

0439 

45 

3311 

3000 

100 

2628 

0000 

50 

3152 

2771 

(Winkler,  B.  1901,  34.  1414.) 


205.69  cc.  H2O  absorb  9.6798  cc.  NO  at  20° 
and  760  mm.  (Hiifner,  Z.  phys.  Ch.  1907, 
59.  420.) 

Sol.  in  cone.  HNO3+Aq. 

100  vols.  HNO3+Aq  of  1.3  sp.  gr.  agitated 
with  NO  gas  take  up  20  vols.  NO.  If  acid  is 
twice  as  strong  or  one^half  as  strong,  the 
quantity  NO  is  proportional  to  the  amount 
of  HNO3.  Very  dil.  HNO3+Aq  absorbs 
scarcely  more  NO  than  pure  H2O.  (Dalton.) 

100  pts.  HNOs+Aq  of  1.4  sp.  gr.  absorb  90  pts.  NO 
(Dalton);  sol.  in  Br2,  and  very  si.  sol.  in  cone.  H2SO.j. 
(Berthelot.) 

1  ccm.  cone.  H2SO4  of  1.84  sp.  gr.  absorbs 
0.035  ccm.  NO;  of  1.50  sp.  gr.,  0.017  ccm. 
NO.  (Lunge,  B.  18.  1391.) 


NITROGEN  OXIDE 


615 


Absorption  of  NO  by  H2SO4+Aq  at  18°  and 
760  mm. 


Absorption  of  NO  by  FeSO4+Aq  at  t°. 
Continued. 


a  =  Coefficient  of  solubility. 

205.69  cc.  of  FeSO4+Aq  contain  0.0296  g. 
Fe. 
Coefficient  of  absorption  =  0.06505. 

H2S04 

a 

H2SC 

4             a 

t° 

Pressure  mm. 

NO  absorbed 
ccm. 

98%       not  constant 
90%           0.0193 
80%           0.0117 

70% 
60% 
50% 

0.0113 
0.0118 
0.0120 

20.05 
20.05 
20.04 
20.00 
20.15 
20.14 

677.5 
655.3 
639.1 
620.2 
600.5 
581.2 

14.30 
14.07 
13.81 
13.39 
13.20 
12.92 

(Tower,  Z.  anorg.  1906,  50.  387.) 

Very  sol.  in  aqueous  solutions  of  ferrous 
salts,  especially  the  sulphate.    (Priestley.) 
1  vol.  FeSO4+Aq  of  1.081  sp.  gr.,  contain- 
ing 1  grain  FeSO4  to  6  grains  H2O,  absorbs  6 
vols.  NO.    (Dalton.) 
Absorption  by  ferrous  salts  +Aq  is  propor- 
tional to  the  amount  of  Fe  present,  irrespec- 
tive of  the  acid  or  concentration  of  the  solu- 
tion.   Between  0°  and  10°,  about  2  mols.  NO 
are  absorbed  for  each  atom  of  Fe;  between 
10°  and  15°,  1  mol.  NO  for  2  atoms  of  Fe; 
and  at  25°,  only  1  mol.  NO  for  21A  to  3  atoms 
of  Fe.     The  amount  of  NO  absorbed  also 
varies  with  the  pressure.    The  sp.  gr.  of  the 
ferrous  salt  solution  is  greater  after  the  ab- 
sorption of  NO  than  before.     The  solutions 
are  decomp.  by  heat,  and  at  100°  all  NO  is 
given  off.    (Gay,  A.  ch.  (6)  5.  145.) 

Absorption  of  NO  by  FeSO4+Aq  at  25°. 

A  =  vol.  H2O  (in  litres)  containing  1  mol. 
FeSO4. 
V  =  vol.  NO  (in  litres)  absorbed. 

205.69  cc.  of  FeSO4+Aq  contain  0.0409  g. 
Fe. 
Coefficient  of  absorption  =  0.06684. 

t 

Pressure  mm. 

NO  absorbed 
ccm. 

20.04 
20.02 
20.00 
20.00 
20.10 

667.6 
650.6 
613.1 
594.6 
577.1 

16.79 
16.65 
15.71 
15.41 
15.32 

205.69  cc.  of  FeSO4+Aq  contain  0.0513  g. 
Fe. 
Coefficient  of  absorption  =0.07981. 

t° 

Pressure  mm. 

NO  absorbed 
ccm. 

20.10 
20.10 
20.08 
20.10 
20.10 
20.10 

644.8 
623.8 
606.4 
589.7 
571.1 
553.1 

18.82 
18.47 
18.02 
17.56 
17.19 
16.95 

205.69  cc.  of  FeSO4+Aq  contain  0.0663  g. 
Fe. 
Coefficient  of  absorption  =0.08059. 

A 

V 

A 

V 

1.2             1. 

1.8            2. 
2.4            2. 
4.82          4. 

47 
01 
55 
40 

7.2 
12,0 
18.6 
36.0 

5.52 
6.46 
8.01 
10.40 

t° 

Pressure  mm. 

NO  absorbed 
ccm. 

20.10 
20.10 
20.10 
20.08 
20.04 
20.00 

697.3 
678.9 
660.4 
638.2 
620.7 
602.5 

21.91 
21.60 
21.18 
20.71 
20.28 
19.87 

(Kohlschutter,  B. 

Absorption  of  NO  bj 

205.69  cc.  FeSO4+Aq 
Coefficient  of  absorpti 

1907,  40 

r  FeSO4+ 

[  contain  ( 
on-0.06C 

877.) 

Aq  at  t°. 

).0221  g.  Fe. 
167  at  20.09°. 

205.69  cc.  of  FeSO4+Aq  contain  0.099  g.  Fe. 
Coefficient  of  absorption  =0.1  1661. 

t° 

Pressure  mm. 

NO  absorbed 
ccm. 

t° 

Pressure  mm. 

VO  absorbed 
ccm. 

20.10 
20.15 
20.20 
20.00 
19.85 
19.85 

649.9 
631.1 
618.4 
603.3 

588.6 
574.2 

34.26 
33.82 
33.26 
.  32.76 
32.34 
31.95 

20.1 
20.1 
20.1 
20.2 
20.05 
20.0 

704 
683 
668 
651 
632 
613 

9 
5 
6 
9 
9 
7 

14.42 
14.10 
13.80 
13.58 
13.15 
12.98 

(Htifner,  Z.  phys.  Ch.  1907,  69.  419.) 

616 


NITROGEN  OXIDE 


Absorption  of  NO  by  NiSO4+Aq  at  t°. 
205.69  cc.  NiSO4+Aq  contain  0.0506  g.  Ni. 
Coefficient  of  absorption  =  0.08311. 

Absorption  of  NO  I 
A  =  vol.  H2O  (in  lii 
FeCl2. 
V—  vol  NO  (in  litr< 

>y  FeCl2+Aq  at  22°. 
bres)  containing  1  mol. 

js)  absorbed. 

t° 

Pressure  mm. 

NO  absorbed 
ccm. 

A 

v 

20.2 
20.2 
20.2 
20.15 
20.14 

654.7 
629.8 
609.5 
591.7 
573.4 

23.00 
22.54 
22.03 
21.65 
21.18 

2.5' 
5.18 
10.35 
20.7 
51.8 

3.30 

4.83 
6.56 
8.32 
11.89 

(Hufner,  I.  c.) 

Absorption  of  NO  by  CoSO4+Aq  at  t°. 
205.69  cc.  CoSO4+Aq  contain  0.0598  g.  Co. 
Coefficient  of  absorption  =  0.09146. 

(Kohlschutter,  B.  1907,  40.  878.) 

Absorption  by  HCl+FeCl2+Aq. 
10.37  1.  30%  HC1  containing  1  mol.  FeCl2 
in  solution  absorb  15.64  1.  NO. 
10.37  1.  10%  HC1  containing  1  mol.  FeCl2 
in  solution  absorb  6.17  1.  NO. 
(Kohlschutter,  I.  c.) 
Absorption  by  salts  -f-Fed2+Aq. 
10.37  1.  sat.  NaCl+Aq  containing  1  mol. 
FeCl2  in  solution  absorb  6.549  1.  NO. 
10.37  1.  sat.  NH4Cl+Aq  containing  1  mol. 
FeCl2  in  solution  absorb  6.549  1.  NO. 
(Kohlschutter,  I.  c.) 

Solubility  of  NO  in  Fe(NO3)2+Aq  at  23°. 
A  =  vol.  H2O  (in  litres)  containing  1  mol. 
Fe(N03)2. 
V  =  vol.  NO  (in  litres)  absorbed. 

f                    Pressure  mm.          NO  absorbed 

20.15                678.3                 23.47 
20.16                653.5                23.01 
20.20                 636.6                 22.55 
20.30                 615.9                 21.99 
20.40                 600.0                 21.56 

(Hufner,  I.  c.) 

Absorption  of  NO  by  MnCl2.4H2O+Aq  at  t°. 
205.69  cc.  MnCl2.4H2O-hAq  contain  0.0697 
g.  Mn. 
Coefficient  of  absorption  =  0.061  11. 

A 

V 

3.25 
6.50 
13.00 
26.00 

2.77 
4.16 
5.54 
6.61 

t°                    Pressure  mm.          NO  ^°rbed 

20.0                   711.96               14.25 
20.05                 686.5                 13.99 
20.2                  657.4                 13.49 
20.3                   638.9                 13.05 
20.45                 621.0                 12.81 

(Kohlschutter,  I.  c.) 

Absorption  of  NO  by  CuCl2+Aq. 
A=vol.  H2O  (in  litres)  containing  1  mol. 
CuCl2. 
V  =  vol.  NO  (in  litres)  absorbed. 

(Hufner,  I.  c.) 

Coefficient  of  absorption  for  FeSO4-fAq  of 
concentration  used  by  Hufner  (Z.  phys.  Ch. 
1907,  69.  417)  =0.180  at  20°.     Hiifner's  re- 
sults are  incorrect  because  he  assumed  that 
the  absorption-coefficient  of  NO  always  had 
the  same  value,  whereas  it  does  not.    NO  is 
reduced  by  FeSO4+Aq.     (Usher,  Z.  phys. 
Ch.  1908,  62.  624.) 
Coefficient  of  absorption  for  CoSO44-Aq 
sat.  at  20°  =  0.0288.     (Usher,  Z.  phys.  Ch. 
1908,  62.  624.) 
Coefficient  of  absorption  for  NiSO4+Aq  of 
the  concentration  used  by  Hufner  (c/.  Z.  phys. 
Ch.  1907,  59.  422)  =0.048  at  20°. 
Coefficient  of  absorption  for  NiSO4+Aq 
sat.  at  20°  =0.0245.    (Usher,  I.  c.) 
Coefficient  of  absorption  for  MnCl2  +Aq. 
sat.  at  20°—  00082      (Usher    Z    phys    Ch 

A 

v 

0.231 
0.277 
0.371 

0.120 
0.098 
0.052 

(Kohlschutter,  I.  c.) 

Absorption  of  NO  by  CuCl2+conc.  HC1. 
A  =  vol.  cone.   HC1  (in  litres)   containing 
1  mol.  CuCl2. 
V  =  vol.  NO  (in  litres)  absorbed. 

A 

V 

A 

v 

0.389 
0.410 
0.840 
1.230 
2.462 

0.801 
0.933 

2.838 
3.426 
3.989 

7.499 
12.500 
18.750 
28.650 

3.931 
3.606 
3.153 
1.976 

1908,  62.  624.) 

(Kohlschutter,  I.  c.) 

NITROGEN  OXIDE 


617 


Absorption  of  NO  by  CuCl2+ acetic  acid. 
A  =  vol.  acetic  acid  (in  litres)  containing  1 
mol.  CuCl2. 

V  =  vol.  NO  (in  litres)  absorbed. 


A 

V 

A 

V 

252 
504 
1269 

51.77 
39.67 
81.60 

0.37 
0.62 
0.925 

0.515 
0.120 
0.000 

(Kohlschtitter,  I.  c.) 

Absorption  of  NO  by  CuCl2+98%  formic 

acid. 

A  =  vol.  98%  formic  acid  (in  litres)  contain- 
ing 1  mol.  CuCl2. 


V  =vol.  JNU  (in  litres)  absorbed. 

A 

V 

27.9 
56.0 
140.0 
280.0 
1400.0 

12.76 
13.17 
14.34 

18.68 
27.29 

(Kohlschtitter,  I.  c.) 

Absorption  of  NO  by  CuCl2+ acetone. 
A=vol.   acetone   (in  litres)    containing   1 
mol.  CuCl2. 

V  =  vol.  NO  (in  litres)  absorbed. 


A 

v 

A 

v 

4.667 
29.16 
58.33 

14.04 
24.01 
24.60 

291.60 
583.20 
1166.40 

40.99 
67.22 
81.96 

(Kohlschtitter,  I.  c.) 

Absorption  of  NO  by  CuCl2  -f  methyl  alcohol. 

A  =  vol.  methyl  alcohol  (in  litres)  contain- 
ing 1  mol.  CuClj. 

V  =  vol.  NO  (in  litres)  absorbed. 


A 

v 

A 

v 

1.60 

8.22 

3.30 
5.60 

20.50 
82.25 

6.15 
4.90 

(Kohlschtitter,  I.  c.) 

Absorption  of  NO  by  CuCl2+ethyl  alcohol. 

A  =  vol.  ethyl  alcohol  (in  litres)  containing 
1  mol.  CuCl2. 

V=vol.  NO  (in  litres)  absorbed. 


A 

V 

A 

v 

1.50 
3.84 
12.80 

8.70 
12.38 
15.43 

38.41 
76.83 
192.10 

18.15 
18.05 
15.92 

(Kohlschtitter,  I.  c.) 


Absorption  of  NO  by  CuBr2+Aq. 
A  =  vol.  H2O  (in  litres)  containing  1  mol. 
CuBr2. 

V  =  vol.  NO  (in  litres)  absorbed. 


(Kohlschtitter,  L  c.) 

Absorption  of  NO  by  CuBr2+ ethyl  alcohol. 

A=vol.  alcohol  (in  litres)  containing  1  mol. 
CuBr2. 

V=vol.  NO  (in  litres)  absorbed. 


A 

2.625 
5.25 
13.12 
43.74 

V 

A 

v 

16.02 
19.26 
20.51 
21.13 

131.20 
262.50 
656.10 

22.23 

23.46 
30.46 

(Kohlschtitter,  I.  c.) 

Sol.  in  stannous  and  chromous  salts+Aq. 

(Peligot.) 

Not  absorbed  by  Fe2(S04)3+Aq.    (Dalton.) 
1  vol.  absolute  alcohol  absorbs  0.31606- 

0.003487t+0.000049t2  vols.  NO  between  0° 

and  25°.    (Bunsen.) 

1  vol.  alcohol  at  t°  and  760  mm.  absorbs  V 
vols.  NO  gas  reduced  to  0°  and  760  mm. 


t° 

V 

"t 

v 

0 

0.31606 

13 

0.27901 

1 

0.31262 

14 

0.27685 

2 

0.30928 

15 

0.27478 

3 

0.30604 

16 

0.27281 

4 

0.30290 

17 

0.27094 

5 

0.29985 

18 

0.26917 

6 

0.29690 

19 

0.26750 

7 

0.29405 

20 

0.26592 

8 

0.29130 

21 

0.26444 

9 

0.28865 

22 

0.26306 

10 

0.28609 

23 

0.26178 

11 

0.28363 

24 

0.26060 

12 

0.28127 

•• 

(Bunsen's  Gasometry.) 

Abundantly  absorbed  by  CS2.  (Friedburg, 
C.  N.  48.  97.) 

Nitrogen  irioxide,  N2O3. 

Sol.  in  H2O  at  0°.  If  large  amt.  of  H2O  is 
present,  the  solution  is  quite  stable  at  ordi- 
nary temp.  (Fremy,  C.  R.  79.  61.) 

Sol.  inHNOa+Aq. 

Sol.  in  cone.  H2SO4  to  form  HNOSO4. 

Sol.  in  ether. 


618 


NITROGEN  OXIDE  STANNIC  CHLORIDE 


Nitrogen    trioxide    stannic    chloride,    N2O3, 

SnCl4. 
Decomp.  by  H2O.    (Weber,  Pogg.  118.  471.) 

Nitrogen  letroxide,  N02  or  N2O4. 

Sol.  in  H2O  at  0°  with  decomp.  Miscible 
with  very  cone.  HNO3.  Absorbed  abundantly 
by  CS2,  CHC13,  and  C6H5C1.  (Friedburg, 
C.  N.  47.  52.) 

Sol.  in  C6H5NO2. 

SI.  sol.  in  H2S+Aq. 

Sol.  in  H2SO4  or  cone.  HNO3+Aq. 

H3PO4  absorbs  some  liquid  NO2.  (Frank- 
land,  Chem.  Soc.  1901,  79.  1362.) 

Nitrogen  pentoxide,  N2O6. 

Very  deliquescent.  Combines  with  H2O  to 
form  HNO3  with  evolution  of  heat. 

Nitrogen  hexoxide,  NO3. 

Decomposes  upon  air  or  with  H2O.  (Haute- 
feuille  and  Chappins,  C.  R.  92.  80,  134;  94. 
1111,  1306.) 

Nitrogen  oxybromide. 
See  Nitrosyl  and  Nitroxyl  bromide. 

Nitrogen  oxychloride. 
See  Nitrosyl  and  Nitroxyl  chloride. 

Nitrogen  oxyfluoride. 
See  Nitrosyl  fluoride  and  Nitroxyl  fluoride. 

Nitrogen  phosphochloride,  P3N3C16. 
See  Nitrogen  chlorophosphide. 

Nitrogen  selenide,  NSe. 

Very  explosive.  Insol.  in  H2O.  Sol.  in 
HNOs+Aq,  and  NaClO+Aq.  (Espenschied, 
A.  113.  101.) 

Insol.  in  H2O,  ether,  absolute  alcohol;  very 
si.  sol.  in  CS2,  C6H6,  and  glacial  acetic  acid. 
Decomp.  by  HC1  or  KOH+Aq.  (Verneuil, 
Bull.  Soc.  (2)  38.  548.) 

Nitrogen  sulphide,  N4S4. 

Insol.  in  H2O.    Decomp.  by  hot  H2O.    SI. 
sol.  in  alcohol,  ether,  wood   alcohol,  oil  of 
turpentine.    Easily  sol.  in  CS2.    Slowly  de- 
comp. by  HCl+Aq  or  KOH+Aq,  rapidly  by 
HNOa+Aq.      15  g.  dissolve  in  1  kilo,  of  CS2. 
(Fordos  and  Gelis,  C.  R.  31.  702.) 
Sol.  in  CHC13.    (Demargay,  C.  R.  91.  854.) 
Sol.  in  warm  glacial  acetic  acid  with  de- 
comp. on  boiling.    (Ruff  and  Geisel,  B.  1904, 
37.  1591.) 

Nitrogen  pentasulphide,  N2S6. 

Sol.  in  ether  and  most  organic  solvents; 
insol.  in  H2O;  fairly  stable  in  ethereal  solu- 
tion, but  decomp.  by  light.  (Muthmann,  Z. 
anorg.  1897,  13.  206.) 


Nitrogen  sulphobromide,  N3S4Br. 

Decomp.  by  boiling  H2O  and  by  dil.  alkalies, 
also  by  boiling  with  alcohol.  (Muthmann, 
B.  1897,  30.  630.) 

N4S4Br4.    Decomp.  by  moist  air.    (Clever, 

B.  1896,  29.  340-341.) 

N4S4Br6.  Decomp.  by  moist  air.  Very 
unstable.  (Clever.) 

N4S6Br2.  Insol.  most  solvents;  unstable. 
(Clever.) 

Nitrogen  sulphochloride,  N4S4C14. 

Unstable  on  air.  Sol.  in  warm  CHC13; 
crystallizes  out  on  cooling.  (Demargay,  C.  R. 
91.  854,  1066.) 

Demarcay  calls  this  comp.  thiazyl  chloride. 

Sol.  in  hot  dry  benzene,  and  in  CC14; 
decomp.  by  moist  air.  (Andreocci,  Z.  anorg. 
1897,  14.  249.) 

N4S6C12.    Partly  sol.  in  H2O.    (Demarcay, 

C.  R.  92.  726.) 

Demargay  calls  this  compound  dithiotetra- 
thiazyl  ^'chloride. 

N2S3C12  =  N2S2,  SC12.  Decomp.  on  air. 
(Fordos  and  Gelis.) 

pemarcay  (C.  R.  92.  726)  calls  this  comp. 
thiodithiazyl  ^chloride. 

N2S4C12.  Sol.  in  H2O  with  subsequent  de- 
comp. More  sol.  than  S  in  CS2.  (Soubeiran, 
A.  ch.  67.  71.) 

Is  a  mixture  of  S2C12  and  N4S4.  (Fordos 
and  Gelis,  C.  R.  31.  702.) 

N3S3C1.  SI.  sol.  in  warm,  insol.  in  cold 
CHC13.  (Demarcay,  C.  R.  92.  726.) 

"  Thio/nazyl  chloride."    (Demargay.) 

N3S4C1.  Sol.  in  H20.  Insol.  in  most 
solvents.  SI.  sol.  in  CHC13.  Easily  sol.  in 
thionyl  chloride.  (Demargay,  C.  R.  91.  854, 
1066.) 

Demargay  calls  the  compound  ihiotri- 
thiazyl  chloride  =  (NS)3  =  S— Cl. 

N4S5C12=2N2S2,  SC12.  Decomp.  on  air. 
(Michaelis.) 

N6S7C12  =  3N2S2,  SC12.  Not  decomp.  on 
air.  Decomp.  by  H2O  containing  ammonia. 


Nitrogen  sulphoiodide,  N3S4I. 

Readily  decomp.   by  H2O. 

and  Seitter,  B.  1897,  30.  627.) 


(Muthmann 


Nitrohydroxylaminic  acid,  H2N2O3. 

Known  only  in  solution.    (Angeli,  Gazz.  ch. 
it.  1897,  27  (2)  357.) 

Barium  nitrohydroxylaminate,  BaN2O3+H2O. 
Ppt.  More  stable  in  the  air  than  the 
sodium  salt.  Not  decomp.  by  prolonged 
boiling  with  H2O.  (Angeli,  Gazz.  ch.  it. 
1896,  26.  17-25.) 

Cadmium   nitrohydroxylaminate,    CdN2O3+ 

H2O. 

As  Ba  salt.    (Angelico  and  Fanara,  Gazz. 
ch.  it.  1901,  31.  (2)  21.) 


NITROSOBROMORUTHENATE  AMMONIA,  SILVER 


619 


Calcium     nitrohydroxylaminate,     GaNjOs+ 

^H20. 
(Angeli,  Gazz.  ch.  it.  1900,  30.  (1)  593.) 

Calcium     nitrohydroxylaminate,     CaN2O3  + 


(Angelico  and  Fanara,  Gazz.  ch.  it.  1901, 
31.  (2)  15.) 

Lead  nitrohydroxylaminate,  PbN203. 
(Angeli,  Gazz.  ch.  it.  1900,  30.  (1)  593.) 

Potassium  nitrohydroxylaminate,  K2N2O3. 

Like  Na  salt.  More  hygroscopic.  (Angeli, 
Gazz.  ch.  it.  1897,  27.  (2)  357.) 

Sol.  in  H2O.  (Angeli,  Gazz.  ch.  it.  1900,  30. 
(1)  593.) 

Silver  nitrohydroxylaminate,  Ag2N2O3. 
Ppt.    (Angeli,  C.  C.  1901,  I.  1192.) 

Sodium  nitrohydroxylaminate,  Na2N2Os. 

Very  sol.  in  H2O.  Pptd.  by  alcohol. 
Aqueous  solution  is  readily  decomp.  by  boil- 
ing. (Angeli,  Gazz.  ch.  it.  1896,  26.  (2)  17.) 

Strontium    nitrohydroxvlaminate,    SrN203  + 

H20. 

(Angeli,  Gazz.  ch.  it.  1900,  30.  (1)  593.) 
+  1J^H2O.     (Angelico  and  Fanara,  Gazz. 

ch.  it.  1901,  31.  (2)  15.) 

Nitroiodic  acid,  I2O4(NO)2 
See  Nitrosoiodic  acid. 

Nitronitrous  acid. 

Platinum  potassium  nitronitrite,  K2Pt(NO2)4. 

N204. 
Decomp.  by  heat.    (Miolati,  C.  C.  1896,  II. 

1088.) 

Nitroplatinous  acid. 
See  Platonitrous  acid. 

Nitroprussic  acid,  H2FeC6N6O+H2O  = 

H2Fe(CN)5NO+H2O. 
Deliquescent.    Easily  sol.  in  H2O,  alcohol, 
or  ether.    (Playfair,  A.  74.  317.) 

Nitroprussides. 

The  alkali  and  alkali-earth  nitroprussides 
are  sol.  in  H2O,  and  the  solutions  are  not 
pptd.  by  alcohol.  The  others  are  mostly  insol. 
in  H2O. 

Ammonium  nitroprusside, 


onum  ntroprusse, 

(NH4)2Fe(CN)5(NO). 


Deliquescent.    Very  sol.  in  H2O;  not  pptd- 
therefrom  by  alcohol.    (Playfair.) 


Barium  nitroprusside,  BaFe(CN)5NO  + 

4H2O. 

Very  sol.  in  H2O. 
+6H2O. 

Cadmium  nitroprusside,  CdFe(CN)5NO. 

Insol.  in  H2O.  Sol.  in  HCl+Aq.  Insol.  in 
dil.  or  cone.  HNO3+Aq  even  when  boiling. 
Not  attacked  by  NH4OH  or  KOH+Aq. 
(Norton,  Am.  Ch.  J.  10.  222.) 

Calcium  nitroprusside,  CaFe(CN)5NO  + 

4H20. 
Very  sol.  in  H2O.    (Playfair.) 

Cobalt  nitroprusside,  CoFe(CN)5NO. 
Ppt.    (Norton,  Am.  Ch.  J.  10.  222.) 
+4H2O. 

Copper  nitroprusside,  CuFe(CN)6NO+2H2O. 
Insol.  in  H2O  or  alcohol. 

Ferrous  nitroprusside,  FeFe(CN)5NO  + 

*H,0(?). 
Insol.  in  H2O. 

Mercurous  nitroprusside,  Hg2Fe(CN)6NO. 

Insol.  in  H2O.  Unstable.  (Norton,  Am. 
Ch.  J.  10.  222.) 

Nickel  nitroprusside,  NiFe(CN)6NO. 
As  the  Co  salt.    (Norton.) 

Potassium    nitroprusside,    K2Fe(CN)6NO  + 

2H20. 

SI.  deliquescent.    Sol.  in  1  pt.  H2O  at  16°. 
K2Fe(CN)5NO,  2KOH.    Very  sol.  in  H2O. 

Silver  nitroprusside,  Ag2Fe(CN)6NO. 

Insol.  in  H2O,  alcohol,  or  HISO3+Aq.  Sol. 
in  NH4OH+Aq. 

Sodium   nitroprusside,    Na2Fe(CN)5NO  + 

2H2O. 

Sol.  in  2%  pts.  H2O  at  16°,  and  in  less  hot 
H2O. 

Zinc  nitroprusside,  ZnFe(CN)6NO. 
Very  si.  sol.  in  cold,  more  in  hot  H2O. 

Nitrosisulphonic  acid. 

Cupric  nitrosisulphonate,  NO^gQ^Cu. 

Decomp.  by  H2O.  (Raschig,  B.  1907,  40. 
4583.) 

Nitrosobromoruthenic  acid. 

Silver  nitrosobromoruthenate  ammonia, 

Ag2Ru(NO)Br5,  NH3. 
Decomp.  by  H2O.     SI.  sol.  in  NH4OH+ 
Aq.     Very  sol.  in  Na2S2O3+Aq.     (Brizard, 
Bull.  Soc.  1895,  (3)  13.  1093.) 


620 


NITROSOBROM03MIC  ACID 


Nitrosobromosmic  acid. 

Potassium  nitrosobromosmate,  K2Os(NO)Br5. 
Stable  in  aqueous  solution.     (Wintrebert, 

A.  ch.  1903,  (7)  28.  132.) 

Nitrosochloroplatinic  acid. 

Potassium  nitrosochloroplatinate, 
KsPtClf(NO). 

Sol.  in  H2O.    (Vezes,  C.  R.  110.  757.) 

Nitrpsochlororuthenic  acid. 

Ammonium  nitrosochlororuthenate. 

(NH4)2Ru(NO)Cl5. 
Sol.  in  H2O.    (Joly,  C.  R.  107.  991.) 
5  pts.  are  sol.  in  100  pts.  H2O  at  25°. 
22    «      «    «     «     «     «      «      «  60°. 
(Howe,  J.  Am.  Chem.  Soc.  1894,  16.  390.) 

Caesium  nitrosochlororuthenate. 
Cs2Ru(NO)Cl5. 

0.20  pt.  is  sol.  in  100  pts.  H2O  at    25°. 

0.56  "    "   "     "     "     "       "     "     100° 

(Howe.) 

+2H2O.  Very  sol.  in  H2O.  105.8  pts.  are 
sol.  in  100  pts.  H2O.  (Howe.) 

Potassium  nitrosochlororuthenate. 

K2Ru(NO)Cl5. 
Sol.  inH2O.    (Joly.) 
12  pts.  are  sol.  in  100  pts.  H2O  at  25°. 
80    "      "      "    "     "      "       "     "  60°. 
(Howe.) 

Rubidium  nitrosochlororuthenate. 

Rb2Ru(NO)Cl5. 

Sol.  in  boiling  H2O  without  decomp. 
0.57  pt.  is  sol.  in  100  pts.  H2O  at  25°. 
2.13  "    "    "     "    "      "      "     "  60°. 
(Howe.) 

Silver  nitrosochlororuthenate  ammonia, 

Ag2Ru(NO)Cl5,  NH3. 
Decomp.  by  H20.    SI.  sol.  in  NH4OH+Aq. 
Very  sol.  in  Na2S2O3+Aq.     (Brizard,  Bull. 
Soc.  1895,  (3)  13.  1092.) 

Nitrosoiodic  acid,  I2O4(NO)2  (?) 

Decomp.  with  H2O,  alcohol,  ether,  or  acetic 
ether.  Slowly  sol.  in  H2SO4.  (Kammerer,  J. 
pr.  83.  65. 

Nitrososulphonic  acid. 

Potassium     dinitrososulphonate,     N2O.OK. 
SO3K. 

Sol.  in  H2O.     Very  unstable.     (Hantzsch, 

B.  1894,  27.  3268.) 

Potassium  nitrosoc&sulphonate,  ON(SO3K)2. 
Sol.  in  H2O.    Very  explosive.     (Hantzsch, 
B.  1895,  28.  996  and  2744.) 


Potassium  nitroso^n'sulphonate,  ON(SO3K)3 

+H2O. 
Sol.  in  H2O.    (Hantzsch,  B.  1895,  28.  2750.) 

Sodium  nitrosofrisulphonate,  NO2(SO3)3Na. 
Decomp.  by  H2O.     (Traube,  B.  1913,  46. 
2521.) 

Nitrososulphuric  acid, 

H2N2S05=H2S03(NO)2. 
Not  known  in  free  state. 

Ammonium  (fa'nitrososulphate, 

(NH4)2(NO)2S03. 

Sol.  in  H2O.  Insol.  in  hot  alcohol.  (Pe- 
louze,  A.  15.  240.) 

Barium ,  Ba(NO)2SO3. 

Sol.  in  H2O.  (Divers  and  Haga,  Chem.  Soc. 
47.  364.) 

Barium  potassium ,  BaK2(SN2O5)2. 

Sol.  in  much  H2O  to  form  a  clear  liquid, 
but  the  solution  gradually  deposits  BaSO4. 
(Hantzsch,  B.  1894,  27.  3271.) 

Cupric  nitrosodteulphate,  Cu(NO)(SO3)2. 
(Sabatier,  Bull.  Soc.  1897,  (3)  17.  787.) 

Lead  cfo'nitrososulphate. 

Insol.  in  H2O.  (Divers  and  Haga,  Chem. 
Soc.  47.  364.) 

Potassium ,  K2(NO)2SO3. 

Decomp.  by  H2O  at  ordinary  temp.  Insol. 
in  alcohol.  (Pelouze,  A.  ch.  60.  160.) 

Sol.  in  about  8  pts.  H2O  at  14.5°.  Less  sol. 
in  presence  of  KOH.  (Divers  and  Haga, 
Chem.  Soc.  1895,  67.  455.) 

Sodium ,  Na2(NO)2SO3. 

More  sol.  than  K  salt.    (Pelouze.) 

SI.  sol.  in  H2O;  very  unstable  moist  or  dry; 

decomp.  by  H2O.     (Divers,  C.  N.  1895,  72. 

266.) 

Nitrososulphurbus  acid. 

Ruthenium  sodium  nitrososulphite, 

O[Ru(SO3)2(NO)Na2]  +2H2O. 
SI.  sol.  in  cold  H2O.     (Miolati,  Gazz.  ch. 
it.  1900,  30.  511.) 

Nitrosulphide  of  iron. 

See  Ferrofeiranitrososulphonic  acid. 

Z^nitrosulphide  of  iron. 

Roussin's  comp.  is  ammonium  ferrohepta- 
nitrososulphonate,  which  see. 


NITRITE,  AMMONIUM 


621 


Nitrosulphonic  acid,  HNSOfi 


.HO 
'NO2 


S02. 


(Lead  chamber  crystals.')  Rapidly  sol.  in 
H2O  with  decomp.  When  brought  into  large 
amount  of  H2O,  no  gas  is  evolved.  (Fremy, 
C.  R.  70.  61.) 

Sol.  in  H2SO4  without  decomp.  Sol.  in  cold 
H2SO4+Aq  of  sp.  gr.  1.7-1.55.  (Weber,  J. 
pr.  100.  37.) 

SI.  sol.  in  H2S04+Aq  of  1.6  sp.  gr.    (Dana.) 

More  difficultly  sol.  in  dil.  than  cone. 
H2SO4+Aq.  (Muller.) 

Potassium  nitrosulphonate,  KOSO2NO2(?). 

Decomp.  by  H2O.  (Schultz-Sellack,  B.  4. 
113.) 

Nitrosulphonic  anhydride  (?),  N2O3,  2SO3 
=  S206(N02)2. 

Rapidly  sol.  in  H2O  with  decomp.  Abund- 
antly soh  in  cold  H2SO4.  (Rose,  Pogg.  47. 
605.) 

Insol.  in  cold,  slowly  sol.  in  warm  H2SO4. 
(Prevostaye,  A.  ch.  73.  362.) 

Nitrosulphonic   chloride,    NO4SC1  = 

NO2SO2C1  (?). 

Decomp.  by  H2O.  Sol.  in  fuming  H2SO4 
without  decomp.  Decomp.  by  cone.  H2SO4. 
(Weber,  Pogg.  123.  333.) 

Dmitrosulphuric  acid. 
See  ZH'nitrososulphuric  acid. 

Nitrosyl  bromide,  NOBr. 

Decomp.  with  cold  H2O.  (Landolt,  A.  116. 
177.) 

Nitrosyl  fnbromide,  NOBr3. 

Decomp.  by  H2O  or  cold  alcohol. 
Miscible  with  ether.  (Landolt,  A.  116. 177.) 
Mixture  of  NOBr  and  Br2.     (Frohlich,  A. 

224.  270.) 

Nitrosyl  platinic  bromide,  2NOBr,  PtBr4. 

Deliquescent.  Decomp.  by  H2O.  (Top- 
see,  J.  B.  1868.  274.) 

Nitrosyl  chloride,  NOC1. 

Decomp.  by  H2O.  Absorbed  by  fuming 
H2S04  without  decomp. 

Nitrosyl  boron  chloride,  NOC1,  BC13. 
See  Boron  nitrosyl  chloride. 

Nitrosyl  platinic  chloride,  2NOC1,  PtCl4. 

Very  deliquescent,  and  sol.  in  H2O  with 
evolution  of  NO.  (Rogers  and  Boye,  Phil. 
Mag.  J.  17.  397.) 


Nitrosyl    thallium    chloride,    2NOC1,    T1C1, 

T1C13. 

Very  deliquescent,  and  sol.  in  H2O  with 
decomp.  (Sudborough,  Chem.  Soc.  59.  657.) 

Nitrosyl  stannic  chloride,  2NOC1,  SnCl4. 

Decomp.  by  H2O,  chloroform,  or  benzene, 
not  by  carbon  disulphide.  (Jorgensen.) 

Nitrosyl  titanium  chloride,  2NOC1,  TiCl4. 
Decomp.  by  H2O.    (Weber,  Pogg.  118.  ,476.) 

Nitrosyl  zinc  chloride,  NOC1,  ZnCl2. 

Very  deliquescent,  and  sol.  in  H2O  with 
evolution  of  NO.  (Sudborough,  Chem.  Soc. 
69.  656.) 

Nitrosyl  chloride  sulphur  Jnoxide,  NOC1,  SO3. 
Decomp.  by  H2O.    Sol.  in  cone.  H2SO4  with 
evolution  of  HC1.    (Weber,  Pogg.  123.  233.) 

Nitrosyl  fluoride,  NOF. 

Sol.  in  H2O.  Solution  decomp.  on  standing 
with  formation  of  NO  and  HNO3.  (Ruff  and 
Stauber,  Z.  anorg.  1905,  47.  190.) 

Nitrosyl  sulphate,  acid,  H(NO)SO4. 
See  Nitrosulphonic  acid. 

Nitrosyl  sulphate,  anhydro,  (NO)2S2O7. 
See  Nitrosulphonic  anhydride. 

Nitrosyl  selenic  acid,  SeO2(ONO)2. 

Decomp.  by  H2O.  (Lenher  and  Mathews, 
J.  Am.  Chem.  Soc.  1906,  28.  516.) 

Nitrosyl  sulphuric  acid,  H(NO)SO4 
See  Nitrosulphonic  acid. 

Nitrous  acid,  HNO2. 

Known  only  in  aqueous  solution. 
See  Nitrogen  Znoxide. 

Nitrites. 

Normal  nitrites,  except  AgNO2,  are  sol.  in 
H2O  and  alcohol;  but,  as  a  rule,  they  are  less 
sol.  than  the  corresponding  nitrates. 

Ammonium  nitrite,  NH4N02. 

Very  deliquescent,  and  sol.  in  H2O. 

H2O  solution  decomp.  at  50°.  (Berzelius.) 
Very  dil.  solution  can  be  evaporated  on  water 
bath  without  decomp.  (Bohlig,  A.  126.  25.) 
Solution  containing  Vioo,ooo  pt.  NH4NO2  can 
be  evaporated  to  %  its  vol.  without  decomp. 
Solution  containing  Vsoo  pt.  gives  a  distillate 
containing  8.6%  of  NH4NO2,  while  residue 
contains  82%  of  original  quantity,  9.4%  being 
lost.  (Schoyen.) 

Very  deliquescent,  sol.  in  H2O;  slowly  but 
easily  sol.  in  alcohol;  insol.  in  ether.  (Soren- 
sen,  Z.  anorg.  1894,  7.  38.) 


622 


NITRITE,  AMMONIUM  BARIUM  CUPRIC 


Ammonium  barium  cupric  nitrite, 

(NH4)2BaCu(NO2)6. 
Ppt.;    decomp.    readily.       (Przibylla, 
anorg.  1897,  15.  424.) 


Z. 


Ammonium  bismuth  silver  nitrite, 

(NH4)2BiAg(N02)6. 
Moderately  sol.  in  H2O.     Rapidly  hydro- 
lyzed  by  H2O.    (Ball  and  Abram,  Chem.  Soc. 
1913,  103.  2120.) 

Ammonium  bismuth  sodium  nitrite, 

2NH4NO2,  Bi(NO2)3,  NaNO2. 
Easily  decomp.     (Ball,  Chem.  Soc.  1905, 
87.  761.) 

Ammonium  cadmium  nitrite  ammonia,  basic, 
2NH4N02,  Cd(N02)2,  Cd(OH)2,  2NH3. 
Decomp.  by  H2O.     (Morin,   C.   R.   100. 
1497.) 

Ammonium  calcium  cupric  nitrite, 

(NH4)2CaCu(NO2)6. 

Ppt.;  decomp.  easily.  Sol.  in  H2O.  SI.  sol. 
in  alcohol.  (Przibylla,  Z.  anorg.  1897,  15. 
423.) 

Ammonium  cobaltic  nitrite,  3(NH4)2O,  Co2O3, 
6N203+1^H20. 

SI.  sol.  in  H2O,  decomp.  in  aq.  solution  on 
heating.  (Rosenheim,  Z.  anorg.  1898,  17.  45.) 

+3H20. 

Somewhat  sol.  in  cold  H2O;  decomp.  by 
boiling.  Decomp.  by  cone.  H2SO4,  not  by 
acetic  or  dil.  mineral  acids.  (Erdmann,  J.  pr. 
97.  405.) 

Ammonium  cupric  lead  nitrite, 

CuPb(NH4)2(NO2)6. 

Stable  at  ordinary  temp.;  sol.  in  HNO3 
with  decomp. 

2.575  pts.  are  sol.  in  100  pts.  H2O  at  20°,  or 
2.51  %'  salt  in  sat.  solution  at  20°.  (Przibylla, 
Z.  anorg.  1897,  15.  420.) 

Ammonium  cupric  strontium  nitrite, 


nonium  cupric  stron 

(NH4)2CuSr(N02)6. 


Ppt.;  sol.  in  H2O  with  decomp.    (Przibylla, 
I.  c.) 

Ammonium  iridium  nitrite. 
See  Iridonitrite,  ammonium. 

Ammonium  lead  nickel  nitrite, 

(NH4)2PbM(N02)6(?). 
Ppt.    (Przibylla,  Z.  anorg.  1897,  15.  433.) 

Ammonium  osmium  nitrite. 
See  Osminitrite,  ammonium. 

Ammonium  osmyl  oxynitrite. 
See  Osmyloxynitrite,  ammonium. 


Ammonium  platinum  nitrite. 
See  Platonitrite,  ammonium. 

Ammonium  rhodium  nitrite. 
See  Rhodonitrite,  ammonium. 

Ammonium     ruthenium     hydrogen     nitrite, 

Ru2H2(NO2)4,  3NH4NO2+3H2O. 
See  Rutheninitrite,  ammonium  hydrogen. 

Barium  nitrite,  Ba(NO2)2+H2O. 
Permanent.    Very  sol.  in  H2O. 

Solubility  in  H2O  at  t°. 


t° 

G.  in  100cc.Ba(NO2)2 

Sp.  gr. 

0 
20 
25 
30 
35 

58 

63 
71 

82 
97 

1.40 
1.45 
1.50 
1.52 
1.61 

(Vogel,  Z.  anorg.  1903,  35.  389. 


100  pts.  H2O  dissolve  at: 

0°        10°  20°      30° 

63.5     69.5  79.5     93  pts,.  Ba(N02)2+H2O, 

40°      50°  60°      70° 

113      136  170      202  pts.  Ba(NO2)2+H2O, 

90°  100°     110° 

331  461      765pts.Ba(NO2)2+H2O. 


80° 
254 


The  sat.  solution  at  17°  contains  40% 
Ba(NO2)2,  and  has  sp.  gr.  17°/0°  =  1.4897. 
(Oswald,  A.  ch.  1914,  (9)  1.  62.) 

100  g.  H2O  at  13.5°  dissolve  64  g.  Ba(N02)2 
+10.2  g.  AgNO2  with  excess  of  AgN02,  and 
75.6  g.  Ba(NO2)2+9.5  g.  AgNO2,  with  ex- 
cess of  AgNO2.  (Oswald.) 

Sol.  in  64  pts.  94%  alcohol;  nearly  insol. 
in  absolute  alcohol.  (Lang,  Pogg.  118.  285.) 

Solubility  in  alcohol +Aq  at  t°. 


t° 

Solvent 

100  ccm.  of  the  sat. 
solution  contain  g. 
Ba(NO2)2+H2O 

19.5 

10%  alcohol 

49.30 

21.0 

20%       " 

29.30 

20.5 

30%       " 

18.41 

20.5 

40%       " 

13.33 

20.5 

50%       " 

9.11 

20.0 

60%       " 

4.84 

19.0 

70%       " 

2.66 

19.5 

80%       " 

0.98 

20.0 

90%       " 

0.00 

20.0 

absolute  alcohol 

0.00 

(Vogel,  Z.  anorg.  1903,  35.  390.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 


NITRITE,  CADMIUM  POTASSIUM 


623 


Barium  caesium  nitrite,  CsBa2(NO2)5. 

Sol.  in  H2O.  (Jamieson,  Am.  Ch.  J.  1907, 
38.  616.) 

Cs2Ba(NO2)4+H2O.  Very  sol.  in  H2O. 
(Jamieson,  Am.  Ch.  J.  1907,  38.  616.) 

Barium  caesium  silver  nitrite,  Cs3AgBa(NO2)6 

+2H2O. 

Decomp.  by  cold  H2O.  (Jamieson,  Am.  Ch. 
J.  1907,  38.  616.) 

Barium  cobaltic  nitrite,  2BaO,  Co2O3,  4N2O3 
+  10H2O. 

Sol.  in  moderately  warm  H20  without  de- 
comp.  but  not  recryst.  therefrom.  (Rosen- 
heim,  Z.  anorg.  1898,  17.  51-54.) 

3BaO,  Co2O3,  6N2O3+H2O.  Ppt.;  very  un- 
stable. Nearly  insol.  in  H2O.  (Rosenheim, 
Z.  anorg.  1898,  17.  47.) 

Barium  cobaltous  potassium  nitrite,  Ba(NO2)2, 

Co(NO2)2,  2KNO2. 
Decomp.  by  H2O.     (Erdmann,  J.  pr.  97. 

385.) 

Barium  cupric  nitrite,  Ba[Cu(OH)(N02)2]2. 

Ppt.  Insol.  in  H2O.  Decomp.  by  H2O. 
Insol.  in  alcohol,  but  slowly  decomp.  by  it. 
(Kurtenacker,  Z.  anorg.  1913,  82.  208.) 

Barium  cupric  potassium  nitrite, 
BaCuK2(NO2)6. 

Stable  when  dry,  easily  decomp.  when 
moist;  sol.  in  H2O  with  decomp. 

45.86  pts.  are  sol.  in  100  pts.  H2O  at  20°,  or 
31.45%  salt  is  contained  in  sat.  solution  at 
20°.  (Przibylla,  Z.  anorg.  1897,  15.  424.) 

Barium  cupric  thallium  nitrite, 

BaCuTl2(NO2)6. 

SI.  sol.  in  H2O.  (Przibylla,  Z.  anorg.  1898, 
18.  461.) 

Barium  iridium  nitrite. 
See  Iridonitrite,  barium. 

Barium  mercuric  nitrite,  2Ba(NO2)2, 

3Hg(N02)2+5H20. 

Very  sol.  in  H2O  and  easily  decomp.  (Ray, 
Chem.  Soc.  1910,  97.  327.) 

Barium  nickel  nitrite,  2Ba(NO2)2,  Ni(N02)2. 

Somewhat  more  easily  sol.  in  H2O  than 
nickel  potassium  nitrite.  (Lang.) 

Barium  nickel  potassium  nitrite,  Ba(NO2)2, 

Ni(NO2)2,  2KNO2. 

SI.  sol.  in  cold,  easily  in  hot  H2O  without 
apparent  decomp.  (Lang.) 

Barium  nickel  thallium  nitrite, 

NiBaTl2(NO2)6 
Ppt.    (Przibylla,  Z.  anorg.  1898, 18.  462.) 


Barium  osmium  nitrite. 
See  Osminitrite,  barium. 

Barium  osmyl  oxynitrite. 
See  Osmyloxynitrite,  barium. 

Barium  potassium  nitrite,  Ba(NO2)2,  2KNO2 

+H20. 

Easily  sol.  in  H2O;  insol.  in  alcohol.    (Lang, 
Pogg,  118.  293.) 

Barium  rhodium  nitrite,  3Ba(NO2)2, 

Rh2(N02)6. 
See  Rhodonitrite,  barium. 

Barium  silver  nitrite,  Ba(NO2)2,  2AgNO2+ 

H2O. 

Resembles  the  potassium  salt.    (Fischer.) 
Less  stable  than  the  Na  salt.    (Oswald.) 


Bismuth  nitrite,  basic,  (BiO)NO2 

Sol.  in  HC1.  (Vanino,  J.  pr.  1906,  (2)  74. 
150.) 

Bismuth  caesium  silver  nitrite,  Cs2BiAg(NO2)6. 
Very  si.  sol.  in  H2O.    Slowly  decomp.  by 
H2O.     (Ball  and  Abram,  Chem.  Soc.  1913, 
103.  2122.) 

Bismuth  potassium  nitrite,  Bi(NO2)3,  3KNO2 

+H20. 

Decomp.  by  H2O.  (Ball,  Chem.  Soc.  1905, 
87.  762.) 

Bismuth  potassium  silver  nitrite, 

K2BiAg(NO2)6. 

Less  sol.  in  H2O  than  NH4  salt.  (Ball  and 
Abram,  Chem.  Soc.  1913,  103.  2121.) 

Bismuth  rubidium  silver  nitrite, 

Rb2BiAg(NO2)6. 

SI.  sol.  in  H2O  with  slow  hydrolysis.  (Ball 
and  Abram.) 

Bismuth  silver  thallous  nitrite,  BiAgTl2(NO2)6  . 
Insol.  in  H2O,  but  decomp.  thereby.    (Ball 
and  Abram.) 

Cadmium  nitrite,  basic,  2CdO,  N2O3. 
Insol.  in  H2O.    (Hampe,  A.  126.  335.) 

Cadmium  nitrite,  Cd(NO2)2+H2O. 

Deliquescent.  Sol.  in  H2O.  (Lang,  J.  B. 
1862.  99.) 

Cadmium  potassium  nitrite,  Cd(NO2)2,  KNO2. 

Easily  sol.  in  H2O.  Very  difficultly  sol.  in 
absolute  alcohol,  and  only  si.  sol.  in  90% 
alcohol.  (Hampe,  A.  125.  334.) 

Cd(N02)2,  2KN02.  Easily  sol.  in  H2O. 
Insol.  in  alcohol.  (Lang,  J.  B.  1862.  99.) 

Cd(NO2)2,  4KNO2.  More  sol.  in  H2O  than 
the  above  salt.  (Lang.) 


624 


NITRITE,  OESIUM 


Caesium  nitrite,  CsNO2. 

Very  hydroscopic.  Very  sol.  in  H2O 
(Ball/Chem.  Soc.  1913,  103.  2130.) 

Caesium  calcium  nitrite,  Cs2Ca(NO2)4+H2O 
Ppt.    (Jamieson,  Am.  Ch.  J.  1907,  38.  617.; 

Caesium  cobaltic  nitrite,  Cs3Co(NO2)6-|-H2O. 

Sol.  in  20,100  pts.  H2O  at  17°.     (Rosen- 

bladt,  B.  19.  2531.) 

Caesium  lead  nitrite,  CsPb(NO2)8+H2O. 

Sol.  in  cold  H2O  without  decomp.  When 
solution  is  heated,  some  basic  lead  salt  sep- 
arates. (Jamieson,  Am.  Ch.  J.  1907,  38.  618.) 

Caesium  lead  silver  nitrite,  Cs3AgPb(NO2)6  + 

2H20. 
Ppt.    (Jamieson.) 

Caesium  silver  nitrite,  CsAg(NO2)2. 
Decomp.  by  H2O.    (Jamieson.) 

Caesium  silver  strontium  nitrite, 

Cs3AgSr(NO2)6+2H2O. 
Partially  decomp.  by  H2O.    (Jamieson.) 

Caesium  strontium  nitrite,  CsSr(NO2)3+H2O. 
Ppt.    Sol.  in  H2O.    (Jamieson.) 

Calcium  nitrite,  Ca(NO2)2+H2O. 

Very  deliquescent.  Insol.  in  dil.  alcohol. 
(Fischer,  Pogg.  74.  115.) 

100  ccm.  of  the  sat.  solution  contain  111.6 
g.  Ca(NO2)2+H2O  at  20.5°.  (Vogel,  Z.  anorg. 
1903,  35.  395.) 

Solubility  in  H2O  at  t°. 


t° 

%Ca(NO2)2 

Solid  phase 

0 

38.3 

Ca(N02)2,  4H20 

18.5 

43 

u 

42 

51.8 

it 

44 
54 

53.5 
55.2 

"  +Ca(N02)2,  H20 
Ca(NO2)2,  H2O 

64 

58.4 

70 

60.3 

" 

73 

61.5 

it 

91 

71.2 

(t 

(Oswald,  A.  ch.  1914,  (9)  1.  32.) 

Sat.  solution  of  Ca(NO2)2+AgN02  con- 
tains 92.4  g.  Ca(NO2)2  and  11.2  g.  AgNO2 
per  100  g.  H?O  at  14°.  (Oswald.) 

Solubility  in  alcohol. 

100  ccm.  of  sat.  solution  in  90%  alcohol 
contain  39.0  g.  Ca(NO2)2+H2O  at  20°. 

100  ccm.  of  sat.  solution  in  absolute  alcohol 
contain  1.1  g.  Ca(N02)2+H2O  at  20°. 
(Vogel.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 


+4H2O.  The  sat.  solution  at  16°  contains 
42.3%  Ca(NO2)2  and  has  sp.  gr.  at  16°/0°  = 
1.4205.  (Oswald,  A.  ch.  1914,  (9)  1.  66.) 

Calcium  cobaltous  potassium  nitrite, 

Ca(NO2)2,  Co(NO2)2,  2KNO2. 
Decomp.  by  H2O.    (Erdmann.) 

Calcium  cupric  potassium  nitrite, 

CaCuK2(NO2)6. 

Ppt.,  insoL  in  alcohol;  sol.  in  H2O  with, 
decomp. 

14.97  pts.  are  sol.  in  100  pts.  H20  at  20°,  or 
13.02  per  cent  of  salt  is  contained  in  sat. 
solution.  (Przibylla,  Z.  anorg.  1897, 15.  422.) 

Calcium  mercuric  nitrite,  Ca(NO2)2,Hg(N02)2 

+5H20. 

Very  sol.  in  H2O.  (Ray,  Chem.  Soc.  1910, 
97.  327.) 

Calcium  nickel  potassium  nitrite,  Ca(NO2)2, 

Ni(N02)2,  2KN02. 

Very  si.  sol.  in  cold,  easily  in  hot  H2O. 
Insol.  in  alcohol.  SI.  sol.  in  dil.  HC2H3O2-J- 
Aq.  (Erdmann.) 

Calcium  osmium  nitrite. 
See  Osminitrite,  calcium. 

Calcium    potassium    nitrite,    CaK(NO2)3  + 

3H2O. 
Sol.  in  H2O.    (Topspe,  W.  A.  B.  73,  2.  112.) 

Deliquescent.    (Lang.) 

Cobaltous  nitrite. 
Known  only  in  solution. 

Cobaltic  lead  nitrite,  3PbO,  Co2O3.  6N2O3-h 

12H20. 

Insol.  in  H2O.  (Rosenheim,  Z.  anorg.  1898, 
17.  48.) 

Cobaltic  lead  potassium  nitrite,  3K20,  3PbO, 

2Co2O3,  10N2O3-f-4H2O. 
Sol.  by  boiling  in  much  H2O.    Sol.  in  hot 
acids  with  evolution  of  N2O3.    (Stromeyer,  A. 
96.  228.) 

Cobaltous  potassium  nitrite,  2Co(NO2)2, 
2KN02+H20. 

Ppt.    (Sadtler.) 

Co(N02)2, 2KN02+H20.    Ppt.    (Sadtler.) 

3Co(NO2)2,  6KNO2+H2O.  Insol.  in  cold, 
>ol.  in  hot  H2O.  SI.  sol.  in  KC2H3O2+Aq. 
'Erdmann,  J.  pr.  97.  397.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
.904,  37.  3602.) 

Cobaltic   potassium  nitrite   (cobalt  yellow), 

Co2(NO2)6,  6KNO2+3H2O. 
Very  si.  sol.  in  cold  H2O.    Insol.  in  alcohol 
md  ether.    Sol.  in  traces  in  CS2.    (St.  Evre, 


NITRITE,  IRON  LEAD  THALLOUS 


625 


C.  R,  36.  552.)  Insol.  in  boiling  cone.  K2SO4, 
KC1,  KNO3,  or  KC2H3O2+Aq. 

Sol.  in  1120  pts.  H2O  at  17°.  (Rosenbladt, 
B.  1886,  19.  2535.) 

Decomp.  when  heated  in  aq.  solution. 
(Rosenheim,  Z.  anorg.  1898,  17.  42.) 

More  sol.  in  NH4C1  or  NaCl+Aq  than  in 
H2O.  (Stromeyer.) 

SI.  decomp.  by  KOH+Aq,  except  when 
very  cone.;  easily  decomp.  by  NaOH  or 
Ba(OH)2+Aq. 

Very  si.  sol.  in  KC2H3O2+Aq,  or  KNO2 
+Aq.  (Fresenius.)  Sol.  in  HCl+Aq. 

Sol.  in  HC2H3O2,  or  H2C204+Aq.  (Stro- 
meyer.) 

Small  quantity  of  HC2H3O2+Aq  does  not 
dissolve.  (Fresenius.) 

Cobaltic  potassium  silver  nitrite, 

KCoAg2(NO2)6,  and  K2CoAg(NO2)6. 
Very  si.  sol.  in  H2O.     Less  sol.  than  Na 
comp.     (Burgess  and  Karum,  J.  Am.  Chem. 
Soc.  1912,  34.  653.) 

Cobaltous  potassium  strontium  nitrite, 

Co(NO2)2,  2KNO2,  Sr(NO2)2. 
Decomp.  by  H2O.     (Erdmann,  J.  pr.  97. 

385.) 

Cobaltic    rubidium    nitrite,    Rb3Co(NO2)6+ 

H2O. 

Sol.  in  19,800  pts.  H2O.  (Rosenbladt,  B. 
19.  2531.) 

Cobaltic  silver  nitrite,  CoAg8(NOa)«. 

Fairly  sol.  in  H2O.  (Cunningham  and 
Perkin,  Chem.  Soc.  1909,  95.  1568.) 

2Ag2O,  Co2O3,  3N2O3+3H2O.  SI.  sol.  in 
H2O;  decomp.  by  boiling  H2O.  (Rosenheim, 
Z.  anorg.  1898,  17.  56.) 

Cobaltic  silver  hydroxynitrite, 

Co2Ag3(OH)3(N02)6. 

SI.  sol.  in  H2O.  (Suzuki,  Chem.  Soc.  1910, 
97.  729.) 

Cobaltic  silver  nitrite  ammonia,  Co2O3,  Ag2O, 

4N2O3,  4NH3. 
See  Cobalt  ammonium  comps. 

Cobaltic  sodium  nitrite,  2Na2O,  Co2O3, 4N2O3. 

Sol.  in  H2O  and  alcohol.  (Rosenheim,  Z. 
anorg.  1898,  17.  50.)  * 

+H2O.  Ppt.  (Sadtler,  Sill.  Am.  J.  (2)  49. 
196). 

3Na2O,  Co2O3,  6N2O3+zH2O.  Sol.  in  H2O; 
decomp.  on  heating;  insol.  in  alcohol.  (Rosen- 
heim, Z.  anorg.  1898,  17.  43.) 

Cobaltic  strontium  nitrite,  2SrO,  Co2O3, 4N2O3 

+  11H.O. 
Ppt.    (Rosenheim,  Z.  anorg.  1898,  17.  54.) 


Cobaltic  thallium  nitrite,  Co2(NO2)6,  6T1NO2. 
Sol.  in  23,810  pts.  H2O  at  17°.     (Rosen- 
bladt, B.  19.  2531.) 

Cobaltic  zinc  nitrite,  2ZnO,  Co2O3,  3N2OS+ 

11H2O. 

Sol.  in  dil.  acetic  acid.  (Rosenheim,  Z. 
anorg.  1898,  17.  56.) 

Cobalt  nitrite  nitrate,  2CoO,  Co2O3,  3N2O3, 

Co(NO3)2+14H2O. 
Ppt.    (Rosenheim,  Z.  anorg.  1898,  17.  58.) 

Cupric  nitrite,  basic,  2CuO,  N2O3. 

(Hampe,  A.  125.  345.) 

Cu(NO2)2,  3Cu(OH)2.  Very  si.  sol.  in  H2O 
or  alcohol.  Easily  sol.  in  dil.  acids  or  am- 
monia, (van  der  Meulen,  B.  12.  758.) 

Cupric  nitrite. 
Known  only  in  solution. 

Cupric  lead  potassium  nitrite,  CuPbK2(NO2)6. 

(van  Lessen,  R.  t.  c.  10.  13.) 

3.056  pts.  are  sol.  in  100  pts.  H2O  at  20°,  or 
2.51%  salt  is  contained  in  sat.  solution  at  20° 
p.  429.  (Przibylla,  Z.  anorg.  1897,  15.  429.) 

Cupric  potassium  strontium  nitrite, 

CuSrK2(NO2)6. 

Sol.  in  H2O  with  decomp.  10.82  pts.  are 
sol.  in  100  pts.  H2O  at  20°,  or  9.77  per  cent 
salt  is  contained  in  sat.  solution  at  20°. 
(Przibylla,  Z.  anorg.  1897,  15.  425.) 

Cupric  rubidium  nitrite,  Rb3Cu(NO2)5. 

Easily  sol.  in  H2O.  Sol.  in  alcohol.  (Kur- 
tenacker,  Z.  anorg.  1913,  82.  206.) 

Cupric  nitrite  ammonia,  Cu(NO2)2,  2NH3+ 
2H2O. 

Sol.  in  little  H2O  with  absorption  of  much 
heat.  Decomp.  by  much  H2O.  (Peligot, 
C.  R.  53.  209.) 

3CuO,  N2O3,  2NH3+H2O.  As  above. 
(Peligot.) 

Iridium  hydrogen  nitrite,  Ir2H6(NO2)i2. 
See  Iridonitrous  acid. 

Iridium  nitrite  with  MNO2. 
See  Iridonitrite,  M. 

Iron  (ferrous)  lead  potassium  nitrite, 

FePbK2(NO2)6. 

Ppt.;  insol.  in  cold  H2O;  stable  at  ordinary 
temp.  (Przibylla,  Z.  anorg.  1897,  15.  439.) 

Iron  (ferrous)  lead  thallous  nitrite, 

FePbTl2(NO2)6. 
Ppt.    (Przibylla,  Z.  anorg.  1898,  18.  463.) 


626 


NITRITE,  LEAD,  BASIC 


Lead  nitrite,  basic,  4PbO,  N2O3+H2O  = 
Pb(OH)NO2,  PbO. 

Sol.  in  143  pts.  H2O  at  23°,  and  33  pts.  at 
100°.  (Chevreul.) 

Sol.  in  1250  pts.  cold  H2O,  and  34.5  pts.  at 
100°.  (Peligot.) 

Sol.  in  cold  HNO3  or  HC2H3O2+Aq. 

Composition  is  3PbO,  N2O3+H2O.  (Meiss- 
ner,  J.  B.  1876.  194.) 

Composition  is  as  above,  (v.  Lorenz,  W.  A. 
B.  84,  2.  1133.) 

3PbO,  N2O3  =  Pb(NO2)2,  2PbO.  Sol.  in 
H2O.  (Bromeis,  A.  72.  38;  v.  Lorenz.) 

2PbO,  N2O3+H2O.  SI.  sol.  in  H2O. 
(Bromeis.) 

+3H2O.    (Meissner.) 

4PbO,  3N2O3-f-2H2O.  Sol.inH2O.  (Meiss- 
ner, J.  B.  1876.  195.) 

Lead  nitrite,  Pb(NO2)2+H2O. 

Easily  sol.  in  H2O.  (Peligot,  A.  ch.  77. 
87.) 

Lead  nickel  potassium  nitrite,  Pb(NO2)2, 
KNO2,  Ni(NO2)2. 

Insol.  in  H2O.  (Baubigny,  A.  ch.  (6)  17. 
111.) 

Ppt.    (Przibylla,  Z.  anorg.  1897,  15.  432.) 

Lead  nickel  thallous  nitrite,  NiPbTl2(NO2)6. 
Ppt.    (Przibylla,  Z.  anorg.  1898,  18.  462.) 

Lead  potassium  nitrite,  4Pb(NO2)2,  6KNO2  + 
3H2O. 

Easily  sol.  in  H2O  and  in  absolute  alcohol. 
(Hampe,  A.  125.  334.) 

Pb(NO2)2,  2KNO2+H2O.  Easily  sol.  in 
H2O.  Insol.  in  alcohol.  (Lang,  J.  B.  1862. 
102.) 

Lead  potassium  silver  nitrite,  K3AgPb(NO2)6 

+2H20. 
Ppt.    (Jamieson,  Am.  Ch.  J.  1907,  38.  619.) 

Lead  nitrite  nitrate. 
See  Nitrate  nitrite,  lead. 

Lithium  nitrite,  LiNO2  +  3^H2O. 

Deliquescent.  Easily  sol.  in  alcohol  and 
H2O.  (Vogel,  Z.  anorg.  1903,  35.  403.) 

Sat.  solution  of  LiNO2+^H2O  in  H2O 
contains  at: 

65°     81.5°     91°      96°     92.5° 

63.8    68.7      72.4    91.8    94.3%  LiNO2. 
(Oswald.) 

+H2O.  Very  sol.  in  H2O,  readily  forming 
supersat.  solutions.  Very  sol.  in  abs.  alcohol. 
(Ball,  Chem.  Soc.  1913,  103.  2133.) 

100  pts.  H2O  dissolve  at: 
0°        10°       20° 
125       156       189  pts.  LiNO2+H2O. 


30° 
242 


40° 
316 


50° 

459  pts.  LiNO2+H2O. 


LiNO2,  H2O+Aq  sat.  at  19°  contains  48.9% 
LiNO2  and  has  sp.  gr.  =  1.3186.  (Oswald,  A. 
ch.  1914,  (9)  1.  61.) 

100  g.  H2O  dissolve  78.5  g.  LiNO2+10.5  g. 
AgNO2  at  14°.  (Oswald.) 

Lithium  mercuric  nitrite,  LiNO2,  Hg(NO2)2  + 

H2O. 

(Ray,  Chem.  Soc.  1907,  91.  2033.) 
4LiNO2,     Hg(NO2)2+4H2O.       Extremely 

deliquescent.    (Ray.) 

Magnesium  nitrite,  Mg(NO2)2-f2H2O. 

Deliquescent,  and  sol.  in  H2O.     Solution 

decomp.  by  boiling.     Easily  sol.  in  absolute 

alcohol.    (Hampe,  A.  125.  334.) 

Insol.  in  absolute  alcohol.    (Fischer.) 
+3H2Q.    Sol.  in  H2O  and  absolute  alcohol. 

Very  deliquescent.     (Vogel,  Z.  anorg.  1903, 

35.  397.) 

Magnesium  osmium  nitrite. 
See  Osminitrite,  magnesium. 

Magnesium  potassium  nitrite. 

Deliquescent,  and  easily  sol.  in  H2O.  Insol. 
in  alcohol.  (Lang.) 

Magnesium  silver  nitrite. 

Sol.  in  H2O  with  decomp.  (Spiegel,  Ch.  Z. 
1895,  19.  1423.) 

Manganous  nitrite. 

Deliquescent,  and  sol.  in  H2O.  (Mitscher- 
lich.)  Not  obtained  in  a  solid  state,  as  the 
solution  decomp.  on  evaporation.  (Lang, 
Pogg.  118.  290.) 

Mercurous  nitrite,  Hg2(NO2)2. 

Sol.  in  H2O  with  partial  decomp.  to  Hg  and 
Hg(NO2)2.  (Ray,  A.  1901,  316.  252.) 

Sol.  in  cold  cone.  HNO3.  Very  slowly  sol. 
in  cold  dil.  HNO3.  (Ray,  Chem.  Soc.  1897, 
71.  339.) 

Decomp.  by  boiling  H2O  and  by  cold  dil. 
H2SO4.  (Ray,  Z.  anorg.  1896,  12.  366.) 

+H2O.  Slowly  decomp.  by  H2O.  (Ray, 
Chem.  Soc.  1897,  71.  340.) 

Mercuric  nitrite,  basic,  Hg(NO2)2,  2HgO  + 
H2O. 

Ppt.    (Lang.) 

12HgO,  5N2O3+24H2O.    (Ray,  Chem.  Soc. 
1897,  71.  341.) 
• 
Mercuric  nitrite,  Hg(NO2)2. 

Deliquescent.  Partly  sol.  in  boiling  H2O, 
but  the  greater  part  is  decomp.  into  HgO  + 
HNO2.  (Ray,  Proc.  Chem.  Soc.  1904,  20.  57.) 

Mercuromercuric  nitrite,  basic, 
a.  9Hg2O,  4HgO,  5N2O3+8H2O. 
/3.  Hg2O,  2HgO,  N2O3+2H2O. 
(Ray,  Chem.  Soc.  1897,  71.  341.) 


NITRITE  POTASSIUM 


627 


Mercuric     potassium     nitrite,      Hg(NO2)2 

Easily  sol.  in  H2O.  Insol.  in  alcohol 
(Lang,  1860.) 

KHg(NO2)3.  Obtained  from  K3Hg(NO2)6 
H20+Aq  containing  a  small  excess  of  KNO2 
Decomp.  by  H2O.  (Rosenheim,  Z.  anorg 
1901,  28.  173.) 

K3Hg(NO2)5+H2O.  Sol.  in  H2O.  For 
mula  of  Lang  is  incorrect.  (Rosenheim,  Z 
anorg.  1901,28.  172.) 

Mercuric  sodium  nitrite,  Na2Hg(NO2)4. 

Very  hydroscopic.  Decomp.  by  hot  H2O 
(Rosenheim,  Z.  anorg.  1901,  28.  173.) 

+2H2O.  Deliquescent.  (Ray,  Chem.  Soc 
1907,  91.  2032.) 

2Hg(NO2)2,  3NaNO2.  Decomp.  by  H2O 
(Ray,  Chem.  Soc.  1907,  91.  2032.) 

Mercuric   strontium  nitrite,   3Hg(NO2)2, 
2Sr(N02)2+5H20. 

Very  sol.  in  H2O.  (Ray,  Chem.  Soc.  1910 
97.  327.) 

Mercuric  nitrite  hydrazine,  Hg(NO2)2,  N2H4. 

Ppt.     Decomp.  by  H2O.     (Hofmann  and 

Marburg,  A.  1899,  305.  215.) 

Nickel  nitrite,  basic,  2NiO,  N2O3. 
Ppt.    (Hampe,  A.  125.  343.) 

Nickel  nitrite,  Ni(NO2)2. 

Sol.  in  H2O  and  alcohol.  (Lang,  J.  B.  1862. 
100.) 

Nickel  potassium  nitrite,  Ni(NO2)2,  4KNO2. 
Moderately  sol.  in  H2O.     (Fischer,  Pogg. 
74.  115.)    Extremely  sol.  in  H2O.     (Hampe, 
A.  125.  346.)    Insol.  in  absolute  alcohol. 

Nickel  potassium  strontium  nitrite,  Ni(NO2)2, 

2KNO2,  Sr(NO2)2. 
SI.  sol.  in  cold,  easily  sol.  in  hot  H2O. 

Nickel  nitrite  ammonia,  Ni(NO2)2,  4NH3. 

Sol.  in  cold  H2O.  Decomp.  on  standing  or 
by  heating.  Insol.  in  alcohol.  Can  be  re- 
crystallized  by  dissolving  in  NH4OH+Aq, 
and  adding  much  absolute  alcohol.  (Erd- 
mann,  J.  pr.  97.  395.) 

Ni(NO2)2,  5NH3.  Decomp.  in  the  air 
giving  Ni(NO2)2,  4NH3.  (Ephraim,  B.  1913, 
46.  3110.) 

Osmium  nitrite,  Os(NO2)3. 
Ppt.    (Wintrebert,  C.  R.  1905,  140.  587.) 

Osmium  nitrite  with  MNO2. 
See  Osminitrite,  M. 

!  Osmyl  nitrite  with  MNO2. 
See  Osmylnitrite,  M. 


Osmyl  oxynitrite  with  MNO2. 
See  Osmyloxynitrite,  M. 

Osmyl  nitrite  ammonia,  Os02(NO2)2,  4NH3. 
(Wintrebert,  A.  ch.  1903,  (7)  28.  56.) 

Palladious  nitrite  with  MNO2. 
See  Palladonitrite,  M. 

Platinous  hydrogen  nitrite,  H2Pt(NO2)4. 
See  Platonitrous  acid. 

Platinous  nitrite  with  MNO2. 
See  Platonitrite,  M. 

Potassium  nitrite,  KNO2. 

Deliquescent.    Sol.  in  H2O. 

Pure  KNO2  is  not  deliquescent.  (Oswald, 
A.  ch.  1914,  (9)  1.  32.) 

Sol.  in  about  l/3  its  wt.  of  H2O.  (Divers, 
Chem.  Soc.  1899,  75.  86.) 

100  pts.  H2O  dissolve  at: 
0°         10°       20°       30°       40° 
281        291       302       313       325  pts.  KNO2, 

50°      60°       70°       80°       90° 
337.5     351       365       380       395  pts.  KNO2, 

100°       110°      120°      130° 

413        432       451       473  pts.  KNO2. 

Bpt.  of  sat.  KNO2-fAq  is  132°  at  758.5  mm. 
pressure. 

(Oswald,  A.  ch.  1914,  (9)  1.  58.) 

Sp.  gr.  of  KNO2+Aq  at  17.5°  containing: 

10         20         30         40%  KN"O,. 
1.049     1.126     1.208 


40%  KN02, 
1.295 


50 
1.377 


60         70 
1.491     1.599 

(Oswald.) 


74.5%  KN"02. 
1.646 


100  g.  H2O  at  13.5°  dissolve  18  g.  KNO2  + 
2.36  g.  AgNO2;  at  25°,  23.1  g.  KNO2+5.3  g. 
A.gN02  with  excess  of  AgNO2. 

100  g.  H2O  at  13.5°  dissolve  276  g.  KNO2  + 
26.3  g.  AgNO2;  at  25°,  279  g.  KNO2+39.3  g. 
A.gNO2  with  excess  of  KNO2.  (Oswald.) 

See  also  under  AgNO2. 

Very  sol.  in  liquid  NH3.     (Franklin,  Am. 

h.  J.  1898,  20.  829.) 

Deliquesces  in  90%  alcohol;  insol.  in  cold 
94%  alcohol.  More  sol.  in  H2O  than  KNO3, 
ut  less  sol.  in  alcohol.  (Fischer.) 

Ppt.  from  its  cone.  aq.  solution  by  the 
addition  of  methyl  alcohol.  Addition  of 
sthyl  alcohol  to  a  cone.  aq.  solution  of  KNO2 
auses  separation  into  two  layers,  of  which 
he  lower  aq.  solution  contains  71.9%  KNO2 
rhile  the  upper  alcoholic  layer  contains  6.9% 
£NO2.  (Donath,  Ch.  Z.  1911,  35.  773.) 

Very  si.  sol.  in  acetone.  (Krug  and  M'El- 
oy,  J.  Anal.  Ch.  6.  184.) 


628 


NITRITE,  POTASSIUM  RHODIUM 


Insol.  in  acetone.     (Eidmann,  C.  C.  1899, 

niOIA-    "Maiiman-n      "R      1  C\C\A     V7     AQ9Q   ^ 

Solubility  in  H2O  at  t°. 

.  iui-1,  i\aumann,  ±>.  lyiM,  of.  lozy.; 
Insol.  in  methyl  acetate.     (Naumann,  B. 

t° 

%  AgNO2 

1909,  42.  3790);  ethvl  acejtate.     (Naumann, 
B.  1904,  37.  3602.) 

1 

0.1589 

15 

0.2752 

OT 

0  412^ 

Potassium  rhodium  nitrite,  6KNO2, 

3s) 

0  fiOlfi 

Rh2(N02)6. 

51 

1  .  0240 

See  Rhodonitrite,  potassium. 

60 

1.3625 

Potassium  ruthenium  nitrite. 
See  Ruthenonitrite,  potassium. 

Potassium   silver  nitrite,    KNO2,    AgNO2  + 


Completely  sol.  in  a  little  H2O,  but  decomp. 
by  more  H2'6.  Sol.  in  KNO2+Aq  without 
decomp.  Insol.  in  alcohol.  (Lang.) 

Potassium  strontium  nitrite,  2KNO2, 

Sr(N02)2. 

Sol.  in  H2O:  insol.  in  alcohol.  (Lang,  Poge. 
118.  293.) 

Potassium  zinc  nitrite,  2KNO2,  Zn(NO2)2+ 
H2O. 

Deliquescent.  Easily  sol.  in  H2O.  (Lang,. 
J.  B.  1862.  101.) 

K3Zn(NO2)6+3H2O.  Very  hydroscopic. 
Decomp.  by  H2O.  (Rosenheim,  Z.  anorg. 
1901,  28.  174.) 

Rhodium  nitrite  with  MNO2. 
See  Rhodonitrite,  M. 

Rubidium  nitrite,  RbNO2. 

Deliquescent;  very  sol.  in  H2O;  si.  sol.  in 
hot  alcohol,  almost  insol.  in  acetone.  (Ball, 
Chem.  Soc.  1913,  103.  2131.) 

Ruthenium  nitrite  with  MNO2. 
See  Ruthenonitrite,  M. 

Silver  nitrite,  AgNO2. 

Sol.  in  120  pts.  cold  H2O  (Mitscherlich),  in 
300  pts.  (Fischer),  and  more  abundantly  in 
hot  H2O. 

1  1.  H2O  dissolves  3.1823  g.  or  0.02067  g. 
mols.  at  18°.  (Naumann  and  Riicker,  B. 
1905,  38.  2294.) 

1  litre  H2O  dissolves  at  — 


0° 

8° 
14° 
16° 
18° 
25° 
33° 


0.0113  mol.  AgNO2 

0.0159 

0.0189 

0.0203 

0.0216 

0.0260 


(Pick  and  Abegg,  Z.  anorg.  1906,  61.  3.) 

1  1.  H2O  dissolves  3.609  g.  AgNO2  at  21°. 
(Oswald,  A.  ch.  1914,  (9)  1.  33.) 


(Creighton  and  Ward,  J.  Am.  Chem.  Soc 
1915,  37.  2335.) 

Solubility  in  AgNO3+Aq  at  18°. 


Mols.  AgNOs  per  1. 
of  the  solution 

Mols.  AgNO2  dissolved 
per  1. 

0. 
0.0026 
0.0052 
0.0103 
0.0207 
0.0413 
0.0827 

0.0207 
0.0198 
0.0190 
0.0169 
0.0144 
0.0117 
0.0096 

(Abegg  and  Pick,  B.  1905,  38.  2573.) 

1  1.  0.2-N  NaNO3+Aq  dissolves  4.956  g 
AgNO2  at  25°.  (Ley  and  Schaefer,  B.  1906 
39.  1263.) 

1  1.  sat.  KNO2+Aq  dissolves  26%  AgNO 
at  13.5°.  (Oswald,  A.  ch.  1914,  (9)  1.  33.) 

Solubility  in  salts +Aq  at  25°. 


Salt 


AgN03 


KNO2 


Cone,  of  the  salt 
mols.  per  1. 


0.00258 
0.00588 
0.01177 
0.02355 
0.04710 


0.00258 
0.00588 
0.01177 
0.02355 
0.04710 


G.AgNOsinlOOg, 
of  solution 


0.4135 


0.3991 
0.3735 
0.3432 
0.2943 

0.2498 


0.3974 
0.3820 
0.3560 
0.3119 
0.2765 


(Creighton  and  Ward,  J.  Am.  Chem.  Soc 
1915,  37.  2336.) 

See  also  under  KNO2. 

AgNO2+NaNO2. 

1  1.  0.02  N-NaNO2+Aq  dissolves  3.185  g, 
AgNO2  at  25°,  0.2-N  NaNO2,  3.016  g.  AgNO2. 
(Ley  and  Schaefer,  B.  1906,  39.  1263.) 

100  g.  H2O  sat.  with  AgNO2  and  Sr(N02)2 
contain  10.9  g.  AgNO2  and  78.3  g.  Sr(N02)2 
at  14°.  (Oswald.) 


NITRITE,  SODIUM 


629 


Very  sol.  in  liquid  NH3.     (Franklin,  Am. 
Ch.  J.  1898,  20.  829.) 
Insol.  in  alcohol. 
Sol.  in  acetone.     (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B,  1904,  37.  4328.) 
100  pts.  acetonitrile  dissolve  23  pts.  at  ord. 
temp.  ;  40  pts.  at  81.6°.    (Scholl  and  Steinkopf, 
B.  1906,  39.  4393.) 
SI.  sol.  in  methyl  acetate.     (Bezold,  Dis- 
sert. 1906.) 
Insol.  in  ethyl  acetate.     (Hamers,  Dissert. 
1906;  Naumann,  B.  1910,  43.  314.) 

Silver  sodium  nitrite,  AgNO2,  NaNO2. 
Completely  sol.  in  a  little  H2O,  but  decomp. 
by  more  H2O.    (Fischer.) 
+  ^H2O.     (Oswald,   A.    ch.   1914,   (9)  1. 

75.) 

Silver  nitrite  ammonia,  AgNO2,  NH3. 
SI.  sol.  in  H2O;  less  sol.  in  alcohol;  nearly 
insol.  in  ether.    (Reychler,  B.  16.  2425.) 
AgNO2,  2NH3.    (Reychler.) 
AgNO2,  3NH3.    Deliquescent.    Sol.inH2O. 
(Reychler.) 

Sodium  nitrite,  NaNO2. 
Not  deliquescent.    Very  sol.  in  H2O. 
More  sol.  in  H2O  than  NaNO3,  but  less  in 
alcohol. 
6  pts.  H2O  dissolve  5  pts.  NaNO2  at  15°. 
(Divers,  Chem.  Soc.  1899,  76.  86.) 
100  g.  H2O  dissolve  83.25  g.  NaNO2  at  15°. 
(Niementowski  and  Roszkowski,  J.  phys.  Ch. 
1897,  22.  146.) 

100  pts.  H2O  dissolve  at  : 
0°       10°        20°        30°         40° 
73       78         84        91.5     98.5  pts.  NaNO2, 

50°     60°        70°        80° 
107      116       125.5      136  pts.  NaNO2, 

90°      100°      110°      120° 
147     160.5      178       198.5  pts.  NaN02. 

B-pt.  of  sat.  NaNO2+Aq  =  128°  at  761.5 
mm.  pressure.    Sat.  solution  at  20°  has  a  sp. 
gr.  =  1.3585.     (Oswald,   A.   ch.  1914,   (9)    1. 

59.) 

Solubility  in  NaNO3+Aq  at  t°. 

Solubility  in  NaNO3+Aq  at  t°.  —Continued. 

t° 

100  pts.  H2O  dissolve 

NaN02 

NaNOs 

21 

84.75 
81.1 
79.7 
73.8 
73.1 
64.2 
46.8 
21.6 
0 

0 
9.6 
23.5 
50.8 
54.5* 
56.7 
62.8 
74.7 
89.3 

52 

108.8 
107.9 
104.3 
101.8 
99.5 
98.0 
97.8 
65.2 
44.2 
27.2 
14.7 
0 

0 
6.7 
20.6 
34.5 
43.2 
62.6* 
82.0 
88.0 
92.9 
101.4 
109 
118 

65 

120.7 
111.5 

108.5 
107.8 
78.3 
49.5 
28.4 
14.7 
0 

0 
34.8 
62.8 
90.6* 
96 
104.1 
113.4 
121  A 
131 

81 

137.1 
125.7 
122.7 
122.6 
79.1 
50.0 
27.2 
0 

0 
38.8 
69.8 
101.0* 
111.5 
121.0 
131.7 
150 

92 

149.7 
141.2 
134.6 
132.3 
60.2 
30.3 
0 

0 
23.6 
57.6 
107.8* 
130.6 
145.0 
163.5 

100  pts.  H2O  dissolve 

t° 

103 

166 
153.3 
148.8 
142.4 
100.0 
60.1 
0 

0 
33.2 
58.8 
116.0* 
126.8 
142.9 
181.2 

NaNOa                     NaNOs 

0                      73                     .0 
68.5                   19 
67.1                   36.3 
64.9                   41.7* 
50.3                   46.8 
30.2                   55.4 
0                       74.2 

*  Both  salts  in  solid  phase. 
(Oswald,  A.  ch.  1914,  (9)  1.  71.) 

630 


NITRITE,  STRONTIUM 


Solubility  in  H2O  is  decreased  by  presence 
of  Na2SO4.  100  pts.  H2O  dissolve  11.8  pts. 
Na2SO4+53.9  pts.  NaNO2.  (Oswald.) 

Very  sol.  in  liquid  NH3.  (Franklin,  Am. 
Ch.  J.  1898,  20.  829.) 

Neither  dissolved  nor  attacked  by  liquid 
NO2.  (Frankland,  Chem.  Soc.  1901,  79. 
1361.) 

Sol.  in  warm  90%  alcohol.  (Hampe,  A. 
125.  336.) 

100  pts.  absolute  methyl  alcohol  dissolve 
4.43  pts.  at  19.5°;  100  pts.  absolute  ethyl 
alcohol  dissolve  0.31  pt.  at  19.5°.  (de  Bruyn, 
Z.  phys.  Ch.  10.  783.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

Strontium  nitrite,  Sr(NO2)2. 

Very  sol.  in  H2O,  and  very  si.  sol.  in  boiling 
alcohol.  (Lang,  Pogg.  118.  287.) 

Easily  sol.  in  90%  alcohol.  (Hampe,  A. 
125.  340.) 

+H2O.  Hydroscopic.  100  ccm.  of  the 
sat.  solution  contain  62.83  g.  Sr(NO2)2+H2O 
at  19.5°.  (Vogel,  2,.  anorg.  1903,  35.  393.) 

100  pts.  H2O  dissolve  at: 
0°        10°       20°      30° 
58.9      67.6      75.5      84  pts.  Sr(NO2)2+H2O, 

40°       50         60°      70° 

94        105       116     130  pts.  Sr(NO2)2+H2O, 

80°       90°      100° 

145        162       182  pts.  Sr(NO2)2+H2O. 

Bpt.  of  sat.  solution  is  112.5°  at  763  mm 
pressure.    The  sat.  solution  at  19°  contains 
39.3%  Sr(NO2)2  and  has  sp.  gr.  at  19°/0C 
1.4461.     (Oswald,  A.  ch.  1914,  (9)  1.  64.) 

Solubility  in  alcohol.  100  ccm.  of  the  solu- 
tion in  90%  alcohol  contain  0.42  g.  Sr(NO2)2 
+H2O  at  20°.  100  ccm.  of  the  solution  in 
absolute  alcohol  contain  0.04  g.  Sr(NO2) 
H2O  at  20°.  (Vogel,  Z.  anorg.  1903,  35.  393.) 

Thallous  nitrite,  T1NO2. 

Sol.  in  H2O.  Ppt.  from  solution  in  H20 
by  absolute  alcohol.  (Togel,  Z.  anorg.  1903 
35.  404.) 

Very  sol.  in  H2O;  insol.  in  alcohol.  (Ball 
Chem.  Soc.  1913,  103.  2131.) 

Zinc  nitrite,  basic,  2ZnO,  N2O3. 
(Hampe,  A.  125.  334.) 

Zinc  nitrite,  Zn(NO2)2+3H2O. 

Deliquescent.  Sol.  in  H2O  and  alcohol 
(Lang,  J.  B.  1862.  99.) 

Nitrous  oxide,  N2O. 
See  Nitrogen  monoxide. 


Nitroxyl  bromide,  NO2Br. 

Decomp.  spontaneously  or  with  H2O. 
Hasenbach,  J.  pr.  (2)  4.  1.) 

Does  not  exist.    (Frohlich,  A.  224.  270.) 

Nitroxyl  chloride,  NO2C1.  . 

Decomp.  by  H2O  without  evolution  of  gas. 

Probably  does  not  exist.  (Geuther,  A.  245. 
98.) 

Nitroxyl  fluoride,  NO2F. 

Absorbed  by  H2O  with  formation  of  HNO3 
and  HF.  Decomp.  by  H2O,  alcohol,  and 
ether.  (Moissan  and  Lebeau,  C.  R.  1905, 
140.  1624.) 

Nitroxypyrosulphuric  acid, 

(HO)S205(N03),  H20. 
Very  deliquescent.     Sol.  in  H2O  with  de- 
comp.    (Weber,  Pogg.  142.  602.) 

Nitryl  chloride,  NO2C1. 
See  Nitroxyl  chloride* 

Octamine  cobaltic  compounds. 

The  formulae  of  the  following  octamine 
cobaltic  compounds  should  be  reduced  one- 
half,  and  they  should  be  classed  with  the 
tetramine  cobaltic  compounds.  (Jorgenseii, 
Z.  anorg.  2.  279.) 

Octamine  cobaltic  carbonate, 
Co2(NH3)8(CO3)6+3H2O. 

Easily  sol.  in  H2O.  (Vortmann  and  Bias- 
berg,  B.  22.  2654.) 

See  Carbonatotetramine  carbonate. 

Co2(NH3)8O3(CO3)4+3H2O.  Rather  diffi- 
cultly sol.  in  H2O. 

chloride  (?).,  Co2(NH3)8  (OH)2C144- 


2H2O. 
Ppt. 

Co2(NH3)8(OH)2Cl4,  2HgCl2. 
Co2(NH3)8(OH)2Cl4,  PtCl4+H2O.     (Vort- 
mann and  Blasberg,  B.  22.  2654.) 


•- —  mercuric  chloride,  Co2(NH3)8Cl6 

3HgCl2+H2O. 

Co2(NH3)8Cl6,  HgCl2.     Difficultly  sol.  ir 
cold  H2O,  decomp.  on  warming.    (Vortmann.] 


chlorosulphite,  Co2(NH3)8(SO3)2Cl! 

+4H20. 

Sol.  in  H2O.     (Vortmann  and  Magdeburg, 
B.  22.  2635.) 


chromate, 

Co2(NH3)8(CrO4)3(H2O)2+2H2O. 
Sol.  in  H2O  or  acetic  acid. 
+8H2O.    Sol.  in  warm  H2O  or  acetic  acid 
Co2(NH3)8(CrO4)2Cr2q7(H2O)2+H2p.  Eas: 
ily  sol.  in  H2O,  from  which  it  is  precipitatec 
by  dil.  HNO3+Aq.    (Vortmann,  B.  15.  5895.] 


OSMIAMIC  ACID 


631 


Octamine  cobaltic  nitrate,  Co2(NH3)8(NO3)6 

+2H20. 

Sol.  in  H2O;  precipitated  by  cone.  HNO3+ 
Aq.    (Vortmann.) 

nitratocarbonate, 

Co2(NH3)8(N03)2(C03)2+H20. 
Less  sol.  than  other  octamine  carbonates, 
(Vortmann  and  Blasberg,  B.  22.  2650.) 
See  Carbonatotetramine  cobaltic  nitrate. 

—  purpureochloride, 

Co2(NH3)8Cl6(H20)2. 


Easily  sol.  in  H2O;  partly  precipitated  from 

~>y  cone.  HC1 
mann,  B.  10.  1451.) 


aqueous  solution  by  cone.  HCl+Aq.     (Vort- 


=  Chlorotetramine  cobaltic  chloride, 
ClCo(NH3)4(OH2)Cl2,  wich  see.  (Jorgen- 
sen,  J.  pr.  (2)  42.  211.) 

— —  — —  purpureomercuric  chloride, 

Co2(NH3)8Cl6(H2O)2,  6HgCl2. 

SI.  sol.  in  cold,  easily  in  hot  H2O.  (Vort- 
mann.) 

=  Chlorotetramine  cobaltic  mercuric  chlo- 
ride. (Jorgensen,  J.  pr.  (2)  42.  211.) 

purpureomercuric  hydroxychloride, 

Co2N8H16(HgCl)4(HgOH)4Cl6. 
Ppt.      (Vortmann    and    Morgulis,    B.    22. 
2647.) 

Co2N8H16(HgOH)8Cl6.    (V.  and  M.) 
Co2N8H16(HgOH)8Cl4(OH)2.  (V.  and  M.) 


• — •  purpureomercuriodide,  basic, 

Co2N8H18(HgOH)6I6. 
(Vortmann  and  Borsbach,  B.  23.  2805.) 


purpureochloroplatinate . 


Very  si.  sol.  in  H2O.     (Vortmann.) 

=  Chlorotetramine  cobaltic  chloroplatinate, 

ClCo(NH3)4(OH2)PtCl6+2H2O.     (Jorgensen, 

J.  pr.  (2)  42.  215.) 


— roseochloride,  Co2(NH3)8Cl6(H2O)2 

+2H2O,  or  4H2O. 

Sol.  in  H2O.    (Vortmann,  B.  15.  1891.) 
See  Roseotetramine  cobaltic  chloride. 

roseomercuric  chloride, 

Co2(NH3)8Cl6(H20)2,  6HgCl2+3H20. 

Ppt.    (Vortmann.) 

— — roseomercuric  hydroxychloride, 

Co2N8H]6(HgCl)6(HgOH)2Cl6. 
(Vortmann  and  Morgulis,  B.  22.  2647.) 
Co2N8H16(HgOH)8Cl6.    (V.  and  M.) 
Co2N8H16(HgOH)8Cl4(OH)2.    (V.  and  M.) 

roseomercuric  iodide, 

Co2N8H2,(HgI)3I6. 

Ppt.     Sol.  in  HC1  or  HNO3.     (Vortmann 
and  Borsbach,  B.  23.  2806.) 


Co2N8H20(HgI)4I6.    Ppt.    (V.  and  B.) 
Co2N8H20(HgI)4l4(OH)2.    Ppt.    (V.andB.) 

Octamine  cobaltic  sulphate, 

Co2(NH3)8(OH)2(S04)2+3H20.  (?). 

Insol.  in  H2O  or  dil.  H2SO4+Aq.  Sol.  in 
moderately  cone.  HCl+Aq.  (Vortmann  and 
Blasberg,  B.  22.  2653.) 

Co2(NH3)8(SO4)3+6H2O.  Sol.  in  H2O. 
(Vortmann.) 

+4H2O.    Easily  sol.  in  H2O. 

See  Roseotetramine  cobaltic  sulphate. 

—  sulphatocarbonate, 

Co2(NH3)8SO4(CO3)2.+3H2O. 
Sol.  in  H2O.    (Vortmann,  B.  10.  1458.) 
See  Carbonatotetramine  cobaltic  sulphate. 
Co2(NH3)8(SO4)2CO3+4H2O.    Sol.  in  H2O. 
(Vortmann  and  Blasberg,  B.  22.  2650.) 


ammonium  sulphite, 

Co2(NH3)8(SO3NH4)6+10H2O. 
See  Octamine  cobaltisulphite,  ammonium. 

Octamine  cobaltisulphurous  acid. 

Ammonium  octamine  cobaltisulphite, 

Co2(NH3)8(SO3NH4)6  +  10H2O. 
Sol.  in  H2O.     (Vortmann  and  Magdeburg, 
B.  22.  2632.) 

Co2(NH3)8(S03)2(S03NH4)2+4H20. 

Ammonium  barium , 

Co2(NH3)8(S03)6Ba2(NH4)2+7H20. 
Ppt.    (V.  and  M.) 


Barium    — • — • 

7H2O, 
Ppt.    (V.  andM.) 


,    Co2(NH3)8(S03)6Ba3+ 


Cobaltic 


Co2(NH3)8(SO3)6Co2+36H2O,  and 
24H20. 


Luteocobaltic , 

Co2(NH3)8(S03)6(NH3)12Co2+8H20. 
Ppt.    (V.  and  M.) 

Octamine  iridium  chloride, 

Ir2(NH3)8Cl6. 

Very,  sol.  in  H2O.    (Palmaer,  B.  22.  16.) 

Octamine  iridium  chlorosulphate, 

Ir2(NH3)8Cl4S04+4H20. 
(Palmaer.) 

Osmiamic  acid,  H2N2Os2O6,  or 

H2N2Os206(?). 

Known  only  in  aqueous  solution,  which  is 
unstable. 


632 


OSMIAMATE,  AMMONIUM 


Ammonium  osmiamate. 

Easily  sol.  in  H2O  or  alcohol.  (Fritzsche 
and  Struve,  J.  pr.  41.  97.) 

Barium  osmiamate,  BaN2Os2O5. 
Moderately  sol.  in  H2O. 

Lead  osmiamate. 

Ppt.    Sol.  in  acids  without  decomp. 

Lead  osmiamate  chloride. 
Ppt. 

Mercurous  osmiamate. 
Ppt. 

Mercuric  osmiamate. 
Ppt. 

Potassium      osmiamate,      K2N2Os2O5,      or 

K2N2Os2O6. 

81.  sol.  in  cold,  much  more  easily  in  hot 
H2O.  81.  sol.  in  alcohol.  Insol.  in  ether. 

Silver  osmiamate,  Ag2N2Os2O6. 

Extremely  si.  sol.  in  H2O  or  cold  HNO3+ 
Aq.  Sol.  in  NH4OH+Aq. 

Sodium  osmiamate. 
Easily  sol.  in  H2O  or  alcohol. 

Zinc  osmiamate,  ZnN2Os2O5. 

Decomp.  by  H2O.  Nearly  insol.  in  NH4OH 
+Aq. 

Osmic  acid,  H2OsO4. 

•  Stable  in  H2O  containing  alcohol.  Sol.  in 
HNO3  or  HCl+Aq.  Not  attacked  by  H2SO4 
-f  Aq.  (Moraht  and  Wischin,  Z.  anorg.  3. 
153.) 

100  g.  H20  dissolve  5,88  g.  H2Os04  at  15°. 
(Squire  and  Cains,  Pharm.  J.  1905,  74.  720.) 

Attacked  by  liquid  NH3.  (Gore,  Am.  Ch. 
J.  1898,  20.  828.) 

Barium  osmate,  BaOsO4+H2O. 

Insol.  in  H2O.    (Glaus,  Pogg.  65.  205.) 

Calcium  osmate,  CaOsO4. 

Insol.  in  H2O.    (Fremy,  J.  pr.  33.  411.) 

Lead  osmate. 

Insol.  in  H2O.    (Fremy.) 

Potassium  osmate,  K2OsO4+2H2O. 

SI.  sol.  in  cold,  much  more  sol.  in  hot  H2O, 
but  is  decomp.  thereby.  81.  sol.  in  KNO2  + 
Aq.  Insol.  in  dil.  or  cone,  alcohol  and  ether. 
Fremy,  A.  ch.  (3)  12.  516.) 

Insol.  in  cone,  saline  solutions.  (Gibbs, 
Am.  J.  Sci.  (2)  31.  70.) 


Sodium  osmate,  Na2OsO4. 

Sol.  in  H2O;  insol.  in  alcohol  and  ether. 
(Fremy,  /.  c.) 

Perosmic  acid. 
See  Perosmic  acid. 

Osminitrous  acid. 

Ammonium    osminitrite,    (NH4)2Os(NO2)5+ 

2H2O. 

Sol.  in  H2O.  Decomp.  when  solution  is 
warmed.  (Wintrebert,  C.  R.  1905,  140.  586.) 

Barium  osminitrite,  BaOs(NO2)5. 
+H2O;  +4H2O.    (Wintrebert.) 

Calcium  osminitrite,  CaOs(NO2)5+4H2O. 
(Wintrebert.) 

Magnesium  osminitrite,  MgOs(NO2)5  + 

4H2O. 
(Wintrebert.) 

Potassium  osminitrite,  K2Os(NO2)5. 

Very  hygroscopic.  Very  sol.  in  H2O. 
Decomp.  by  HC1,  HBr  and  HI.  (Wintrebert, 
A.  ch.  1903,  (7)  28.  135.) 

Silver  osminitrite,  Ag2Os(NO2)5+2H2O. 

81.  sol.  in  H2O  with  partial  decomp.  (Win- 
trebert, C.  R.  1905,  140.  586.) 

Sodium  osminitrite,  Na2Os(NO2)6-f-2H2O. 
Sol.  in  H2O.    (Wintrebert.) 

Strontium  osminitrite,  SrOs(NO2)5+2H2O. 
(Wintrebert.) 

Zinc  osminitrite,  ZnOs(NO2)5+3^H2O. 
(Wintrebert.) 

Osmyloxynitrous  acid. 

Ammonium    osmyloxynitrite, 

(NH4)2OsO3(NO2)2. 

Decomp.  by  boiling  cone.  HC1  and  by  KOH 
+Aq.  (Wintrebert,  A.  ch.  1903,  (7)  28.  107.) 

Barium     osmyloxynitrite,     BaOsO3(NO2)2  + 
4H2O.    (Wintrebert.) 

Potassium  osmyloxynitrite,  K2OsO3(NO2)2  + 

3H20. 

81.  sol.  in  cold  H2O.  Aqueous  solution  de- 
comp. slowly.  Sol.  with  decomp.  in  dil.  KOH 
+Aq.  (Wintrebert.) 

Silver  osmyloxynitrite,  Ag2OsO3(NO2)2+H2O. 
(Wintrebert.) 


OSMIUM  OXIDE 


633 


Strontium   osmyloxynitrite,   SrOsO3(NO2)2  + 
3H2O.    (Wintrebert.) 

Osmylnitrous  acid. 

Potassium  osmylnitrite,  K2OsO2(NO2)4. 

Decomp.  by  H2O  and  by  excess  of  KOH+ 
Aq.  (Weinland,  A.  ch.  19C3,  (7)  28.  54.) 

Osmisulphurous  acid. 

Potassium  osmisulphite,   [Os(H2O)(SO3)5]K6 

+4H20. 
Ppt.    (Rosenheim,  Z.  anorg.  1899,  21.  144.) 

Potassium  hydrogen  osmisulphite, 

[Os2(H2O)(SO3)n]KuH3+5H2O. 
Sol .  in  H  2O  without  decomp .    ( Rosenheim . ) 
[Os(SO3)6]K6H2+2H2O.    Sol.  in  H2O  with- 
out decomp.    (Rosenheim.) 

Sodium  osmisulphite,  [Os(SO3)6]Na8+8H2O. 

Only  si.  sol.  in  H2O. 

[Os(H2O)(SO3)5]Na6+4H2O.    Ppt. 

[OsO(SO8)4]Na«-r-3H2O.  Ppt.  (Rosen- 
heim.) 

Osmium,  Os. 

When  finely  divided  and  not  ignited  to  a 
very  high  temperature,  Os  is  sol.  in  HNO3+ 
Aq  or  aqua  regia.  When  ignited  it  is  not  at- 
tacked by  any  acid. 

Insol.  in  liquid  NH3.  (Gore,  Am.  ch.  J. 
1898,  20..  828) 

Osmium  ammonium  comps. 
See — 

Oxyosmiumamine  comps.,  OsO(NH3)2X. 
Oxyosmiumcfa'amine  comps.,  OsO2(NH3)4X2. 

Osmium  bromide  with  MBr. 
See  Bromosmate,  M. 

Osmium  ^chloride,  OsCl2. 

Deliquescent.  Sol.  in  little,  but  decomp.  by 
more  H2O,  with  pptn.  of  Os.  Sol.  in  cone, 
alkali  chlorides +Aq  with  combination  and 
partial  decomp.  (Berzelius.) 

Sol.  in  alcohol  and  ether. 

Insol.  in  H2O.  Insol.  in  HC1  and  H2SO4 
SI.  sol.  in  HNO3  and  aqua  regia.  Slowly  sol 
in  strong  alkali.  Insol.  in  liquid  C12.  Insol 
in  alcohol  and  formaldehyde.  (Ruff,  Z.  anorg 
1910,  65.  455.) 

Osmium  trichloride,  OsCl3. 

Hydroscopic.  Sol.  in  cone.  H2SO4,  HC1  anc 
cone.  HNO3.  Sol.  in  alkali  and  in  NH4OH 
Insol.  in  liquid  C12.  Easily  sol.  in  alcohol 
SI.  sol.  in  ether.  (Ruff,  Z.  anorg.  1910,  65 
453.) 

+3H2O.  Sol.  in  H2O.  (Moraht  and  Wis- 
chin,  Z.  anorg.  3.  153.) 


Osmium  tefrachloride,  OsCl4. 

Sol.  in  a  little  II 2O,  but  decomp.  by  further 
addition  of  that  solvent.  Sol.  in  cone.  HC1+ 
Aq. 

Osmium  trichloride  with  MCI. 
See  Chlorosmite,  M. 

Osmium  tetracbloride  with  MCI. 
See  Chlorosmate,  M. 

Osmium  sodium  chloride,  Na2OsCl6+2H2O. 
Very  sol.  in  H2O  and  in  alcohol.     (Rosen- 
heim, Z.  anorg.  1899,  21.  133.) 

Osmium  tefrafluoride,  OsF*. 

Sol.  in  H2O.    (Ruff,  B.  1913,  46.  948.) 

Osmium  fterrafluoride,  OsF6. 

Decomp.  by  H2O  and  cone.  H2SO4.  Sol.  in 
NaOH+Aq.  (Ruff,  B.  1913,  46.  945.) 

Osmium  octofluoride,  OsF8. 

Sol.  in  H2O,  but  is  somewhat  hydrolyzed. 
Sol.  in  cone.  H2SO4  with  decomp.  Sol.  in 
NaOH+Aq.  (Ruff,  B.  1913,  46.  944.) 

Osmium  worcohydroxide,  OsO,  zH2O. 

Insol.  in  H2O.  SI.  sol.  in  KOH+Aq. 
Slowly  but  completely  sol.  in  acids.  (Ber- 
zelius.) 

Osmium  dihydroxide,  OsO2,  H2O. 

Sol.  in  HCl+Aq  while  still  moist.  Insol. 
in  H2SO4  or  HNO3+Aq. 

+2H2O.  Sol.  in  HC1,  HNO3,  or  H2SO4+ 
Aq  while  still  moist.  (Glaus  and  Jacoby.) 

Osmium  sesgwihydroxide,  Os2OeH6. 

Sol.  in  acids,  and  partly  sol.  in  KOH+Aq. 
(Glaus  and  Jacoby.) 

Osmium  iodide,  Osl4. 

Extremely  deliquescent.  Sol.  in  H2O  of 
alcohol,  but  solution  is  unstable.  (Moraht 
and  Wischin,  Z.  anorg.  3.  153.) 

Osmium  potassium  nitrosochloride, 

K2Os(NO)Cl5. 

Stable  in  aqueous  solution.  Only  si.  at- 
tacked by  hot  HNO3.  (Wintrebert,  A.  ch. 
1903,  (7)  28.  132.) 

Osmium  monoxide,  OsO. 

Insol.  in  H2O  or  acids.    (Glaus  and  Jacoby.) 

Osmium  dioxide,  OsO2. 
Insol.  in  H2O  or  acids. 

Osmium  sesgiuoxide,  Os2O3. 

Insol.  in  acids.    (Glaus  and  Jacoby.) 


634 


OSMIUM  OXIDE 


Osmium  ^noxide,  "  Osmic  acid,"  OsO3. 
See  Osmic  acid. 

Osmium  tetroxide,  "  Perosmic  acid,"  OsO4. 

Slowly  but  abundantly  sol.  in  H2O.  Sol.  in 
alcohol  and  ether  with  gradual  decomposition. 
Sol.  in  NH4OH+Aq,  the  solution  undergoing 
decomposition  on  heating. 

Osmium  oxide  ammonia,  OsO2,  2NH3+H2O. 
See  Oxyosmiumamine  hydroxide. 

Osmium  oxysulphide,  Os3S7O5+2H2O. 

Unstable. 

OsSO3+l^H2O.  Insol.  in  H2O.  (v. 
Meyer,  J.  pr.  (2)  16.  77.) 

Os2O2S2+H2O.  Decomp.  and  dissolved  by 
HNO3,  HC1,  or  H2SO4+Aq.  (Moraht  and 
Wischin,  Z.  anorg.  3.  153.) 

Osmium  sulphide,  Os2S3  (?). 

(Berzelius.) 

Min.  Laurite.  Insol.  in  all  acids,  even  in 
aqua  regia. 

Osmium  cfa'sulphide,  OsS2. 

SI.  sol.  in  H2O;  not  more  sol.  in  alkali 
hydrates  or  carbonates +Aq.  Insol.  in  al- 
kalies after  drying.  (Fremy,  A.  ch.  (3)  12. 
521.) 

Osmium  tefrasulphide,  OsS4+^H2O. 

Insol.  in  alkali  sulphides,  carbonates,  or 
hydroxides +Aq.  Sol.  in  cold  dil.  H,NO3+ 
Aq.  (Glaus.) 

Osmocyanhydric  acid,  H4Os(CN)6. 

Easily  sol.  in  H2O  and  alcohol.  Insol.  in 
ether.  (Martius,  A.  117.  361.) 

Barium  osmocyanide,  Ba2Os(CN)6+6H2O. 
Easily  sol.  in  H2O  and  dil.  alcohol.    (M.) 

Barium  potassium  osmocyanide, 

BaK2Os(CN)6+3H2O. 
Efflorescent.    SI.  sol.  in  cold,  easily  in  hot 
H2O. 

Ferric  osmocyanide,  Fe4[Os(CN)6]3+zH2O. 
Insol.  in  H2O. 

Potassium  osmocyanide,  K4Os(CN)6+3H2O. 
Moderately  sol.  in  boiling,  less  in  cold  H2O. 
Insol.  in  alcohol  and  ether. 

Osmosyl  ammonium  comps. 
See  Oxyosmium  amine  comps. 

Osmyl  pottasium  bromide,  K2OsO2Br4+ 
2H20. 

Same  properties  as  the  chloride.  (Wintre- 
bert,  A,  ch.  1903,  (7)  28.  94.) 


Osmyl  potassium  chloride,  K2OsO2Cl4. 

Very  sol.  in  H2O.  Solution  is  stable  only 
in  the  presence  of  a  small  amt.  of  HC1.  De- 
:Comp.  by  hot  cone.  HC1. 

+2H2O.  As  the  anhydrous  salt.  (Wintre- 
bert,  A.  ch.  1903,  (7)  28.  86.) 

Osmyl  c&tetramine  comps. 
See  Oxyosmium  famine  comps. 

Oxamidosulphonic  acid. 
See  Hydroxylamine  wonosulphonic  acid. 

Oximidosulphomc  acid. 
See  Hydroxylamine  efosulphonic  acid. 

Oxyamidosulphonic  acid. 
See  Hydroxylamine  sulphonic  acid. 

Oxyammonium  salts. 

See  Hydroxylamine  salts. 

Oxycobaltamines,  acid  comps. 

(Maquenne,  C.  R,  96.  344.) 

Are  anhydrooxycobaltamine  comps.,  which 
see.  (Vortmann,  M.  ch.  6.  404.) 

Oxycobaltamine  chloride, 

Co2(NH3)100(gg)Cl4. 

(Vortmann,  M,  ch.  6.  404.) 
Co2(NH3)10O2Cl4,   HC1+3H2O.     Is  anhy 
drooxycobaltamine  chloride,  which  see. 

chloronitrate  hydrochloride, 

Co2(NH3)10(OH)(O.OH)(NO3)2Cl2, 
4HC1+3H2O. 

Is  anhydrooxycobaltamine  chloronitrate, 
which  see. 


chlorosulphate, 


,  4HC1. 


Easily  decomp. 

-  iodide,  Co2(NH3)10  (0(OH))14- 

SI.  sol.  in  H2O.     Decomp.  by  much  H2O. 
(Vortmann.) 

-  nitrate,  Co2(NH3)10(OH)(O.OH)(NO3)4 
+H20. 

Decomp.  by  H2O. 

Co2(NH3)10(OH)(O.OH)(N03)4,  HNO3+ 
2H2O.    Decomp.  by  H2O. 

—•  —  nitratosulphate, 

Co2(NH3)]0(OH)(O.OH)(SO4)(NO3)2, 
4HNO3. 
Decomp.  at  once  by  H2O. 


OXYGEN 


635 


Oxycobaltamine  sulphate, 

Absorption  of  O  by  HaO.  —  Continued 

Co2(NH3)10O2(SO4)2,  H2SO4+H2O. 

t 

g 

0i 

Very  si.  sol.  in  H2O  with  decomp.;  more 
easily  sol.  in  acidified  H2O.     Sol.  in  acids. 
(Maquenne,  C.  R.  96/344.) 

14 
15 
16 

0.3486 
3415 
3347 

0.3431 
3358 

3288 

CoatNHsho/Q^Q^)  (SO4)2+3H2O. 

17 

3283 

3220 

\                          / 

18 

3?20 

3155 

Co2(NH3)10(0^I))(HS04)4.     Decomp. 

19 
20 

3161 
3102 

3093 
3031 

violently  by  H2O. 

21 

3044 

2970 

22 

2988 

2911 

Oxygen,  O2. 

23 

2934 

2853 

100  vols.  H2O  absorb  4.6  vols.  O  gas  at  ord.  temp. 

24 

2881 

2797 

(Otto-Graham.) 
Sol.  in  27  pts.   H2O  at  ord.  temp.      (Pelouze  and 
Fremy.) 

25 
26 

2831 

2783 

2743 
2691 

100  vols.  H2O  dissolve  0.925  vol.  O.     (Gay-Lussac.) 

27 

2736 

2641 

1  vol.  H2O  at  t°  and  760  mm.  absorbs  V  vols. 
O  gas,  reduced  to  0°  and  760  mm. 

28 
29 
30 

2691 
2649 
2608 

2592 
2545 
2500 

t°           V 

t°              V 

t°             V 

31 

2572 

2459 

32 

(}  £  c\f-r 

0     0.04114 

7     0.03465 

14    0.03034 

O^faf 

33 

2503 

2380 

1      0.04007 

8     0.03389 

15     0.02989 

34 

2471 

2342 

2      0.03907 

9     0.03317 

16     0.02949 

35 

2440 

2306 

3      0.03810 

10     0.03250 

17     0.02914 

36 

2410 

2270 

4     0.03717 

11     0.03189 

18     0.02884 

37 

2382 

2236 

5      0.03628 

12     0.03133 

19     0.02858 

38 

2355 

2203 

6      0.03544 

13     0.03082 

20    0.02838 

39 

2330 

2171 

40 
41 

2306 
2280 

2140 
2107 

(Bunsen's  Gasometry.) 

Coefficient  of  absorption  of  O  by  H2O  = 

42 

2256 

2075 

0.041  15-0.0010899t  +0.000022563t2.       (Bun- 

43 

2232 

2043 

sen  and  Pauli,  A.  93.  21.) 

44 

2209 

2012 

Coefficient  of  absorption  of  O  in  H2O  at 

45 

2187 

1981 

6.4°  =  0.041408;  at  12.6°  =  0.036011.    (Timofe- 

46 

2166 

1952 

jew,  Z.  phys.  Ch.  6.  148.) 

47 

2145 

1922 

Absorption  of  O  by  H2O.     Pi  =  "  solubility," 
i.  e.,  the  amount  of  gas  (reduced  to  0°  and 
760  mm.)  which  is  absorbed  by  1  vol.  of 
the  liquid  when  the  barometer  indicates 
760  mm.  pressure;  j8  =  coefficient  of  ab- 
sorption, i.  e.,  amount  absorbed  by  the 
liquid  when  the  pressure  of  the  gas  itself 
without  the  tension  of  the  liquid  amounts 

48 
49 
50 
52 
54 
56 
58 
60 
62 

2126 
2108 
2090 
2057 
2026 
1998 
1971 
1946 
1921 

1894 
1865 
1837 
1782 
1728 
1674 
1619 
1565 
1508 

to   760  mm.;    /3i=j8760~f.   when  f=va- 

64 

1897 

1450 

760 

66 

1874 

1392 

por  tension  of  solvent  at  t°. 

68 

pyf\ 

1853 

1332 

70 

1833 

1270 

t° 

ft 

ft 

72 

*J  A 

1815 

1208 

0 

0.04890 

0.04860 

74 
76 

1799 
1785 

1144 
1078 

1 

4759 

4728 

78 

1772 

1010 

2 

4633 

4601 

80 

1761 

0939 

3 

4512 

4479 

82 

1752 

0865 

4 

4397 

4362 

84 

1743 

0788 

5 

4286 

4250 

86 

1736 

0707 

6 

4181 

4142 

88 

1729 

0622 

7 

4080 

4040 

90 

1723 

0532 

8 

3983 

3941 

92 

1717 

0437 

9 

3891 

3847 

94 

1712 

0337 

10 

3802 

3756 

96 

1708 

0231 

11 

3718 

3670 

98 

1704 

0119 

12 

3637 

3587 

100 

7001 

0000 

13 

3560 

3507 

(Winkler,  B.  24.  3609.) 

OXYGEN 


Absorption  of  O  by  H2O  at  t°  and  760  mm. 

/3  =  coefficient  of  absorption. 

? 

ft 

t° 

0 

t° 

|8 

0 

0.04961 

23 

0.03006 

46 

0.02163 

1 

4838 

24 

2956 

47 

2139 

2 

4720 

25 

2904 

48 

2115 

3 

4606 

26 

2855 

49 

2092 

4 

4496 

27 

2808 

50 

2070 

5 

4389 

28 

2762 

51 

2049 

6 

4236 

29 

2718 

52 

2029 

7 

4186 

30 

2676 

53 

2009 

8 

4089 

31 

2635 

54 

1990 

9 

3994 

32 

2596 

55 

1972 

10 

3903 

33 

2558 

56 

1955 

11 

3816 

34 

2521 

57 

1938 

12 

3732 

35 

2486 

58 

1922 

13 

3651 

36 

2452 

59 

1907 

14 

3573 

37 

2419 

60 

1893 

15 

3497 

38 

23  87 

65 

1832 

16 

3425 

39 

2356 

70 

1787 

17 

3357 

40 

2326 

75 

1752 

18 

3292 

4J 

2297 

80 

1726 

19 

3230 

42 

2269 

85 

1707 

20 

3171 

43 

2241 

90 

1693 

2] 

3114 

44 

2214 

95 

1684 

22 

3059 

45 

2188 

100 

1679 

(Bohr  and  Bock,  W.  Ann.  (2)  44.  318.) 

Coefficient  of  absorption  of  O  by  H2O  be- 

tween   0°    and    30°  =  0.04890—  0.0013413t  + 

0.0000283t2—  0.00000029534t3.  (Winkler,  I.  c.) 

Solubility  in  H2O  at  25°  =0.03080;  at  15°  = 

0.03630.     (Geffcken,  Z.  phys.  Ch.  1904,  49. 

269.) 

Absorption  of  O2  by  distilled-  H2O  at  t°. 

a  =  ccm.  of  O2  absorbed  by  1  1.  of  H2O  at 

t°  and  760  mm. 

t°             a 

t° 

a 

t° 

a 

0      49.24 

17 

33.21 

34 

25.19 

1       47.94 

18 

32.58 

35 

24.85 

2      46.65 

19 

32.01 

36 

24.52 

3      45.45 

20 

31.44 

37 

24.20 

4      44.31 

21 

30.91 

38 

23.89 

5      43.21 

22 

30.38 

39 

23.59 

6      42.15 

23 

29.86 

40 

23.30 

7      41.15 

24 

29.38 

41 

23.02 

8      40.19 

25 

28.90 

42 

22.75 

9       39.28 

26 

28.42 

43 

22.49 

10      38.37 

27 

27.94 

44 

22.24 

11       37.51 

28 

27.51 

45 

22.00 

12       36.75 

29 

27.08 

46 

21.77 

13       35.98 

30 

26.65 

47 

21.55 

14      35.26 

31 

26.27 

48 

21.34 

15       34.55 

32 

25.90 

49 

21.14 

16       33.88 

33 

25.54 

50 

20.95 

(Fox,  Trans.  Faraday  Soc.  1909,  5.  74.) 

Solubility  in  H2O  at  various  pressures. 

V  =  volume  of  the  absorbing  liquid. 
P  =  Hg-pressure  in  metres. 
X  =  coefficient  of  solubility. 


V 

t° 

P 

X 

33.320  ccm. 

23° 

0.9595 

0.02937 

1.0941 

0.02939 

1.2883 

0.02938 

1.4976 

0.02935 

1.7638 

0.02939 

2.0838 

0.02931 

2.5011 

0.02928 

3.0402 

0.02909 

3.8675 

0.02886 

4.2504 

0.02872 

4.6301 

0.02855 

5.1360 

0.02832 

5.6973 

0.02818 

6.1857 

0.02797 

6.7343 

0.02772 

7.3051 

0.02741 

7.7138 

0.02729 

8.1406 

0.02708 

32.003  ccm. 

25.9° 

0.8611 

0.02848 

0.9808 

0.02849 

1.0833 

0.02846 

1.2039 

0.02842 

1.4112 

0.02845 

1.6602 

0.02847 

2.3854 

0.02831 

2.6482 

0.02826 

2.8995 

0.02816 

3.2883 

0.02803 

3.9133 

0.02798 

4.2720 

0.02785 

4.6905 

0.02776 

5.0559 

0.02762 

5.6141 

0.02740 

6.0120 

0.02734 

6.5687 

0.02719 

7.1056 

0.02687 

7.4729 

0.02676 

8.1889 

0.02645 

(Cassuto,  Phys.  Zeit.  1904,  5.  236.) 


Solubility  of  O  in  H2O  at  25°  =  0.0294. 
(Findlay  and  Creighton,  Bioch.  J.  1911,  5. 
294.) 

Coefficient  of  absorption  for  H2O=  0.03398 
at  15°;  0.03375  at  15.3°;  0.03330  at  16.2°. 
(Miiller,  Z.  phys.  Ch.  -1912,  81.  494.) 


OXYGEN 


637 


Solubility  in  H2O  at  t°. 

1 760  =  solubility  of  atmospheric  O2  in  H2O  at 
760  mm.  and  t°. 


0 

1 

2 

3 

4 

5 

6 

7 

8 

9 

10 

11 

12 


1760 


10.26 
9.99 
9.73 
9.48 
9.25 
9.02 
8.80 
8.59 
8.39 
8.20 
8.02 
7.84 
7.67 


13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 


1760 


51 

36 
21 
07 
93 


6.80 
6.67 
6.55 
6.43 
6.32 
6.21 
6.10 
6.00 


(Carlson,  Zeit.  angew.  Ch.  1913,  26.  714.) 

Solubility  of  atmospheric  O2  in  mixtures  of 
distilled  H2O  with  sea  water  diminishes  regu- 
larly with  the  proportion  of  sea  water  present. 
(Clowes,  J.  Soc.  Chem.  Ind.  1904,  23.  359.) 

No.  of  ccm.  of  O2  absorbed  by  1 1.  of  sea  water 
from  a  free  dry  atmosphere  of  760  mm. 
pressure. 


Cl 

per 
1000 

G 

4 

8 
12 
16 
20 


.299 


10 

9.83 
9.36 

8. 
8. 
7.97 


908 
437 


8° 


8.407 


26 

8.858.04 
8.457.687 

04 

64 
7.23 


7.33 
6.97 
6.62 


12° 


.68 
7. 

.04 
6. 

6.43 
11 


366 


746 


10° 


7 

.80 
.52 
.24 
5.96 
5.69 


20° 


075 


576.145.75 
5.53 
5.31 


5.91 
67 


6.33 

5.'825.445. 
5.565.204 
5.31 


28° 


.86 
4.954.62 


(Fox,  Trans.  Faraday  Soc.  1909,  5.  77.) 

For  O  absorbed  from  the  air,  see  also  air, 
atmospheric,  p.  1. 

Absorption  of  O2  by  acids +Aq. 
M  =  content  in  gram-equivalents  per  litre. 
S  =  solubility. 

HNO,+Aq. 


M 

S25° 

S  15° 

0.492 
0.494 
1.00 
1.008 

1.88 
1.901 

0.03021 
0.03016 
0.02954 
0.02963 
0.02853 

0.03478 
0.03490 
0.03354 
0.03365 
0.03175 
0.03166 

Absorption  of  O2  by  acids+Aq. — Continued. 
HCl+Aq. 


M 

S25° 

S  15° 

0.578 
0.579 
1.170 
1.176 
1.736 
1.982 

0.02963 
0.02960 
0.02817 
0.02833 
0.02733 
0.02674 

0.03431 
0.03410 
0.03217 
0.03109 
0.03069 
0.02988 

H2S04 


+Aq. 


0.489 
0.527 
0.977 
1.017 
1.896 
1.829 
2.947 
3.512 
4.951 
5.293 


S  25° 


0.02887 
0.02875 
0.02757 
0.02745 
0.02545 
0.02577 
0.02285 
0.02198 

0.01918 


S  15° 


0.03366 
0.03375 
0.03210 
0.03217 
0.02886 
0.02930 
0.02584 
0.02399 
0.02174 
0.02067 


(Geffcken,  Z.  phys.  Ch.  1904,  49.  269.) 

Absorption  of  O2  by  H2SO4+Aq  at  t°. 
a  =  coefficient  of  absorption. 


Normality  of  the  acid 


0 

4.9 
8.9 
10.7 
20.3 
24.8 
29.6 
34.3 
35.8 


20.9 
20.9 
20.9 
21.2 
21.1 
21.5 
20.8 
20.9 
21.2 


0.0310 
0.0195 
0.0155 
0.0143 
0.0119 
0.0103 
0.0117 
0.0201 
0.0275 


(Bohr,  Z.  phys.  Ch.  1910,  71.  49.) 


Absorption  of  O2  by  NaOH-fAq. 

M  =  content  in  gram-equivalents  per  litre. 
S  =  solubility. 


M 

825° 

S  15° 

0.559 
0.601 
1.033 
1.059 
2.077 
2.089 

0.02434 
0.02424 
0.02020 
0.01991 
0.01295 
0.01272 

0.02777 
0.02784 
0.02291 
0.02262 
0.01479 
0.01456 

638 


OXYGEN 


Absorption  of  O2  by  KOH+Aq. 


M 

S  25° 

S  15° 

0.577 
0.579 
1.157 
1  .  170 

0.02447 
0.02435 
0.01920 
0.01914 

0.02791 
0.02791 
0.02191 
0.02181 

(Geffcken,  Z.  phys.  Ch.  1904,  49.  270.) 

NaCl+Aq  with  a  chlorine  content  of  1,930 
per  100,000  dissolved  82.9%  of  the  amount 
of  O2  dissolved  by  distilled  H2O  alone. 
(Clowes,  J.  Soc.  Chem.  Ind.  1904,  23.  359.) 

Absorption  of  O2  by  salts +Aq. 
M  =  content  in  gram-equivalents  per  litre. 
S  =  solubility. 

Absorption  of  O=  by  K2^°4+Aq. 


M 

S25° 

S  15° 

0.499 
0.506 
0.968 
0.970 

0.025^8 
0.02530 

0.02096 

0.02944 
0.02922 
0.02395 
0.02377 

Absorption  of  O2  by  NaCl+Aq. 


M 

S25° 

S  15° 

0.530 
0.535 
1.02C 
1.034 
1.880 
1.890 
1.921 

0.02598 
0.02604 
0.02226 
0.02202 

0.01663 
0.01654 

0.03045 
0.030521 
0.02601 
0.02557 
0.01898 
0.01904 
0.01869 

(Geffcken,  Z.  phys.  Ch.  1904,  49.  270.) 

Solubility  of  O2  in  NaCl+Aq. 
Data  indicate  cc.   O2   dissolved   per  1. 
760  mm.  and  0°. 


at 


t° 

NaCl  +Aq 
1  g.  mol.  per  1. 

NaCl  +Aq 
2  g.  mol.  per  I. 

NaCl  +Aq 
sat.  at  20° 

0 
5 
10 
15 
20 
25 
30 

6.50 
5.80 

5.25 

4.77 
4.39 
4.06 
3.76 

3.14 
2.84 
2.59 
2.41 
2.25 
2.13 
2.01 

1.27 
1.22 
1.17 
1.12 
1.07 
•1.02 
0.97 

(Winkler,  Z.  anorg.  1911,  24.  342.) 

Solubility  of  O2  in  KCN+Aq  at  209. 
%  KCN  1          10        20        30        50 

Coeff.  of  abs.  0.029  0.018  0.013  0.008  0.003 
(McLaurin,  J.  S.  C.  I.  1893,  63.  737.) 


1  vol.  alcohol  absorbs  0.28397  vol.  O  at  all 
temperatures  between  0°  and  24°.    (Bunsen.) 

Absorption  by  alcohol  (99.7%)  at  t°. 
0  =  coefficient  of  absorption; 
Pi  =  solubility.    (See  p.  635.) 


t° 

ft 

ft 

0 

0.23370 

0.22978 

1 

0.23296 

0.22878 

2 

0.23222 

0.22777 

3 

0.23149 

0.22675 

4 

0.23077 

0.22572 

5 

0.23005 

'  0.22469 

6 

0.22934 

0.22365 

7 

0.22863 

0.22260 

8 

0.22793 

0.22155 

9 

0.22724 

0.22047 

10 

0.22656 

0.21937 

11 

0.22588 

0.21827 

12 

0.22521 

0.21715 

13 

0.22455 

0.21601 

14 

0.22389 

0.21484 

15 

0.22324 

0.21365 

16 

0.22259 

0.21245 

17 

0.22195 

0.21122 

18 

0.22132 

0.20994 

19 

0.22069 

0.20862 

20 

0.22007 

0.20733 

21 

0.21946 

0.20600 

22 

0.21886 

0.20459 

23 

0.21826 

0.20317 

24 

0.21767 

0.20172 

(Timofejew,  Z.  phys.  Ch.  6.  151.) 
Solubility  of  O2  in  alcohol  at  20°  and  760  mm. 


Wt.  % 
alcohol 

Vol.% 
abs.  O2 

wt.  % 

alcohol 

Vol.  % 
abs.  02 

0.0 
9.09 
16.67 
23.08 

28.57 

2.98 

2.78 
2.63 
2.52 
2.49 

33.33 
50.0 
66.67 
80.0 

2.67 
3.50 
4.95 
5.66 

(Lubarsch,  W.  Ann.  1889,  (2)  37.  525.) 
Solubility  of  O2  in  methyl  alcohol  at  t°. 


t° 

l. 

-  t° 

1. 

0 
5 
10 
15 
20 

0.31864 
0.30506 
0.29005 
0.27361 
0.25574 

25 
30 
40 
50 

0.23642 
0.21569 
0.16990 
0.11840 

(Levi,  Gazz.  ch.  it.  1901,  31.  II,  513.) 


Solubility  of  O2  in  ether  at  0°  =  0.4235;  at 
10°  =0.4215.  (Christoff,  Z.  phys.  Ch.  1912, 
79.  459.) 


OXYMERCURIAMMONIUM  CARBONATE 


639 


Solubility  of  O2  in  acetone  at  t°. 

Absorption  of  O2  by  glucose  +Aq. 
t°  =  temp.  of  the  solution. 
P  =  %  glucose  in  the  solution. 
£  t°  =  coefficient  of  absorption  at  t°. 
£  20°  =  coefficient  of  absorption  at  20°. 

t° 

l. 

t° 

1. 

0 
5 
10 
15 
20 

0.2997 
0.2835 
0.2667 
0.2493 
0.2313 

25 
30 

40 
50 

0.2127 
0.1935 
0.1533 
0.1057 

t° 

p 

/3t° 

£20° 

21.2 
21.5 
19.9 
20.5 
21.7 

10.84 
20.7 
33.8 
51.9 

58.84 

0.02650 
0.02202 
0.01814 
0.01378 
0.01221 

0.02690 
0.02250 
0.01815 
0.01390 
0.01250 

(Levi,  Gazz.  ch.  it.  1901,  31.  II,  513.) 

Absorption  of  O2  by  chloralhydrate+Aq. 

t°  =  temp.  of  the  solution. 
P  =  %  chloralhydrate  in  the  solution. 
/3  t°  =  coefficient  of  absorption  at  t°. 
/3  15°  =  coefficient  of  absorption  at  15°. 
/3  20°  =  coefficient  of  absorption  at  20°. 


(Muller.) 

Absorption  of  O2  by  sucrose +Aq. 
t°=temp.  of  the  solution. 
P  =  %  sucrose  in  the  solution. 
j9  t°  =  coefficient  of  absorption  at  t°. 
15°  =  coefficient  of  absorption  at  15C 


t° 

P 

ftt° 

ft  15° 

t° 

P 

ftt° 

ft  15° 

18.3 
16.9 
15.4 

22.9 
28.0 
36.6 

0.02759 
0.02690 
0.02590 

0.02940 
0.02800 
0.02560 

15.3 
16.2 

0.03375 
0.03330 

0.03400 
0.03397 

16.6 
12.8 
16.2 
15.9 
17.2 
16.9 

38.6 
51.3 
58.44    • 
70.0 
80.85 
80.9 

0.02402 
0.02439 
0.02350 
0.02659 
0.03200 
0.03140 

0.02477 
0.02339 
0.02407 
0.02710 
0.03300 
0.03250 

16.0 
15.6 
16.6 
15.6 
16.2 
17.2 

12.1 
24.38 
28.44 
42.96 
49.25 
50.0 

0.02911 
0.02367 
0.02113 
0.01582 
0.01348 
0.01302 

0.02969 
0.02396 
0.02181 
0.01600 
0.01380 
0.01359 

ft  20° 

(Muller.) 

20.0 
21.0 
21.0 
20.4 
•    21.8 
21.0 
22.2 

16.9 
32.0 
52.9 
61.08 
65.5 
71.4 
78.0 

0.02795 
0.02443 
0.02375 
0.02390 
0.02500 
0.02680 
0.03090 

0.02795 
0.02495 
0.02325 
0.02410 
0.02580 
0.02730 
0.03280 

Abundantly  absorbed  by  oil  of  turpentine. 
Oil  of  turpentine  absorbs  its  own  vol.  O  when 
exposed  two  weeks  to  the  air,  but  does  not 
give  it  off  on  boiling.    (Brandes.) 
Absorbed  by  other  oils,  but  this  is  decom- 
position rather  than  absorption,  as  the  oils 
are  oxidized.    (See  Storer's  Diet.) 

(Muller,  Z.  phys.  Ch.  1912,  81.  499.) 

100  vols.  arterial 
O.    (Magnus.) 

blood  dissolve  10-13  vols. 

Coefficient  of  absorption  for 

petroleum  = 

0.202  at 

20°:  0.229 

at  10°.     (Gniewasz  and 

Absorption  of  O2  by  glycerine  +Aq. 

Walfisz,  Z.  phvs.  Ch.  1.  70.) 

t°  =  temp.  of  the  solution. 
P  =  %  glycerine  in  the  solution. 
ft  t°  =  coefficient  of  absorption  at  t°. 
ft  15°  =  coefficient  of  absorption  at  15°. 

The  author  examined  the  solubility  of  O2 
and  N2  at  low  temp,  in  alcohols,  ethers,  ace- 
tone, CHC13,  petroleum,  benzene  and  various 
inorganic  liquids;  at  low  temp,  the  solubility 
of  the  N2  increases  at  the  same  rate  as  that  of 

i'L          /~\ 

//~il         J         s~*i 

T?     i  onn    1  9 

1      /MO   \ 

t° 

P 

ftt° 

ft  15° 

, 

12.2 
12.5 

20.5 
25.0 

0.02904 
0.02654 

0.02742 
0.02521 

Oxyrfimercuriaminonium  bromate, 

(NHg2OH2)BrO3. 

14.6 

37.3 

0.02038 

0.02022 

(Rammelsberg,  Pogg.  56.  82.) 

13.5 

45.0 

0.01800 

0.01744 

12.4 

52.0 

0.01623 

0.01570 

-  carbonate,  (NHg2OH2)2CO3  +  ^H2O. 

12.1 
13.3 

71.5 

88.5 

0.01010 
0.00906 

0.00950 
0.00886 

Insol.  in  H2O.    Decomp.  by  HCl+Aq  only 
when  cone.    Not  decomp.  by  boiling  KOH  + 

Aq.    Decomp.  by  KI  or  K2S+Aq.     (Hirzel.) 

(Muller.) 

+H20 

As  above.    (Hirzel.) 

640 


OXYMERCURIAMMONIUM  CHLORIDE 


Oxycfomercuriammonium  chloride, 

(NHg2OH2)Cl. 

Is  dzmercuriammonium  chloride,  NHg2Cl  + 
H2O,  which  see. 

oxy^nmercuriammonium  chloride, 

(NHg,OH,)Cl,  (NHg302H2)Cl  (?). 
Insol.  in  H2O.  Easily  sol.  in  dil.  HCl+Aq. 
More  difficultly  sol.  in  very  dil.  H2SO4  or 
HNO3+Aq.  .Insol.  in  cone.  H2SO4.  Sol.  in 
boiling  NH4Cl+Aq,  or  (NH4)2SO4+Aq.  De- 
comp.  by  KOH+Aq.  (Schmieder.) 

—  chromate,  (NHg2OH2)2CrO4. 
Not  decomp.  by  KOH+Aq.    (Hirzel,  J.  B. 
1852.  421.) 

mercuric  chromate,  (NHg2OH2)2CrO4, 

4HgO,  3CrO3. 

Decomp.  by  HNO3  without  going  into  solu- 
tion. Easily  sol.  in  HC1.  (Hirzel.) 

Composition  is  (NHg2OH2)2O,  2Cr()3, 
3[(NH4)20,  2Cr203]  =  (NHg2OH2)2Cr2O7, 
3(NH4)2Cr2O7.  (Hensgen,  R.  t.  c.  5.  187.) 

Probably  (NHg2)oCr2O7,  3(NH4)2Cr2O7  + 
2H20. 

—  fluoride,  acid,  (NHg2OH2)F,  HF. 
(Finkener,  Pogg.  110.  632.) 
Probably  NHg2F,  HF+H2O. 

hydroxide,  (NHgoOH2)OH  =  NHg2OH  + 

H2O. 

(Millon's  base.)  SI.  sol.  in  H2O,  especially 
if  warm.  Sol.  in  13,000  pts.  H2O  at  17°,  and 
1700  pts.  at  80°.  Insol.  in  alcohol  or  ether. 
(Gerresheim,  A.  195.  373.) 

+H2O.  Insol.  in  H2O  or  alcohol.  Sol.  in 
traces  in  NH4OH+Aq.  Not  decomp.  by  cold 
KOH+Aq;  si.  decomp.  if  hot.  (Millon.) 

ammonium  iodate,  (NHg2OH2)IO3, 

2NHJO3. 
Insol.  in  H2O.    (Millon,  A.  ch.  (3)  18.  410.) 

-  iodide,  (NHg2OH2)I. 

Sol.  in  warm  HCl+Aq.  Not  decomp.  by 
boiling  KOH+Aq.  Sol.  in  warm  KI+Aq. 
(Rammelsberg,  Pogg.  48.  170.) 

Correct  formula  is  NHg2I+H2O.  (Ram- 
melsberg.) 

nitrate,  (NHg2OH2)NO3. 

Insol.  in  H2O;  not  decomp.  by  boiling 
KOH+Aq.  Sol.  in  cold  HCl+Aq,  from 
which  it  is  precipitated  by  H2O.  SI.  sol. 
without  decomp.  in  HNO3  or  H2SO4+Aq 
Easily  sol.  in  NH4OH+Aq.  (Soubeiran.) 

Is  dimercuriammonium  nitrate,  NHg2NO3. 
(Pesci,  Gazz.  ch.  it.  20.  485.) 

ammonium    nitrate,    NHg2OH2)NO3, 

2NH4NO3+H2O. 

Decomp.  by  H2O.    Kane,  A.  ch.  72.  242.) 
Is  dimercufiammonium  ammonium  nitrate 

NHg2NO3,  2NH4NO3+2H2O.    (Pesci.) 


Oxycfo'mercuriammonium  oxide, 

(NHg,OH,),0. 

Insol.  in  H2O  or  alcohol;  not  attacked  by 
boiling  cone.  KOH  +  Aq.  Sol.  in  hot  NH4NO3 
+  Aq,  NH4C1  +  Aq,  (NH4)2SO4  +  Aq, 
NH4C2H3O2+Aq,  (NH4)2C2O4+Aq.  (Mil- 
Ion,  A.  ch.  (3)  18.  397.) 


—  mercuric  phosphate,  Hg(NHg2OH2)PO4. 
Insol.  in  H2O.    Slowly  sol.  in  hot  HNO3  + 

Aq;  not  decomp.  by  boiling  with  KOH+Aq, 
but  by  KI  or  K2S+Aq.  Sol.  in  HCl+Aq  or 
much  hot  (NH4)2HPO4+Aq.  (Hirzel.) 

—  mercuric  sulphite,  (NHg2OH2)2SO3. 
HgS03. 

Insol.  in  H2O.  Sol.  in  much  (NH4)2SO3  + 
Aq.  Sol.  in  HCl+Aq  with  decomposition. 
Insol.  in  boiling  KOH+Aq.  (Hirzel.) 

-  sulphate,  (NHg2OH2)2SO4. 

Sol.  in  traces  in  H2O.  Easily  sol.  in  HC1  or 
HNO3+Aq.  (Kane.) 

Insol.  in  HNO3+Aq.    (Hirzel.) 

Slowly  sol.  in  boiling  cone.  H2SO4.  (Hir- 
zel.) 

Insol.  in  cone.,  easily  sol.  in  dil.  H2SO4+ 
Aq.  (Schmieder,  J.  pr.  76.  147.) 

Moderately  sol.  in  much  (NH4)2SO4  or  boil- 
ing NH4Cl+Aq.  Not  decomp.  by  boiling 
KOH+Aq.  (Hirzel.) 

Easily  decomp.  by  boiling  with  dil.  KOH  + 
Aq.  (Schmieder.) 

Does  not.  exist.    (Pesci.) 

2NH3,  2HgO,  SO3. 

See  Di'mercuriammonium  sulphate. 

Oxytfn'mercuriammonium  chloride, 

(NHg302H2)Cl  (?). 
Insol.  in  H2O. 

-  nitrate,  (NHg3O2H2)NO3. 

Sol.  in  cold  HCl+Aq,  from  which  it  is  pre- 
cipitated by  NH4OH+Aq.  Sol.  in  NH4OH  + 
Aq  without  decomp.  Not  decomo.  by  H2SO4 
or  warm  KOH+Aq.  (Pagenstecher.) 

Does  not  exist.  (Pesci,  Gazz.  ch.  it.  20. 
485.) 

Oxyfrimercuridi'ammonium  sulphate, 

2NH3,  3HgO,  SO3. 
See  Tnmercuriammomum  sulphate. 

Oxyfrimercurioxydimercuriammonium 
sulphate, 


Completely  sol.  in  NH4Cl+Aq,  or 
(NH4)2SO4+'Aq.  Sol.  in  dil.  or  cone.  HC1  + 
Aq,  and  very  dil.  H2SO4+Aq.  Insol.  in  HNO3 
+Aq  or  cone.  H2SO4.  (Schmieder.) 

Does  not  exist.    (Pesci.) 


OZONE 


641 


Oxyfeframercuriammonium  mercuric 
nitrate  (?),  2(NHg4O2)NO3,  HgNO3  (?) 

Completely  insol.  in  HNO3+Aq.     Sol.  in 
warm  HCl+Aq.    Slowly  decomp.  by  boilin 
KOH-f-Aq.      Graduallv    sol.    in    hot    cone 
NH4NO3+Aq.    (Hirzel.) 

Does  not  exist.     (Pesci,  Gazz.  ch.  it. 
485.) 

Oxynitrosulphonic  anhydride, 

a  ~    ^NO2      /9N 


Sol.  in  H2O  with  decomp.     (Weber,  Pogg 
123.  339.) 

Oxyosmiumamine  hydroxide  (Osmo- 
sylcfa'amine  hydroxide), 

OsO(NH3OH)2. 

Insol.  in  H2O.     SI.  sol.  in  acids.     Sol.  in 

KOH+Aq.     When  moist,  sol.  in  NH4OH  + 

Aq. 

Oxyosmiumdi'amine  chloride  (OsmylteJr- 

amine  chloride),  OsO2(N2H6Cl)2. 
SI.  sol.  in  cold,  more  easily  in  hot  H2O 
Insol.  in  NH4Cl+Aq.     (Gibbs,  Am.  Ch.  J 
3.  233.) 

—  chloroplatinate,  OsO2(N2H6Cl)2,  PtCl4. 
SI.  sol.  in  H2O.    (Gibbs.) 


hydroxide,  OsO2(N2H6OH)2. 

Known  only  in  solution. 

—  nitrate,  OsO2(N2H6NO3)2. 

sulphate,  OsO2(N2H6)2SO4+H2O. 

(Gibbs,  Am.  Ch.  J.  3.  233.) 

Oxyphosphuretted  hydrogen  (?), 

P4H(OH). 

P4O  of  Leverrier,  and  Goldschmidt  has  this 
formula  according  to  Franke  (J.  pr.  (2)  35. 
341).  Decomp.  slowly  by  H2O  or  alkalies. 
Forms  potassium  salt,  P4H(OK),  sol.  in  H2O. 

-  hydroiodide,  P4H(OH),  HI. 
Decomp.  at  80°. 

/Se6<zmoxyplatisulphuric  acid,  Pt2O3, 

3SO3,  SO4H2  +  11KH2O. 
Sol.  in  H2O.     (Blondel,  A.  ch.  1905,  (8)  6. 
113.) 

Barium  sesgiuoxyplatisulphate,  Pt2O3,  3SO3, 

SO4Ba+8H2O. 
Very  sol.  in  H2O.    (Blondel.) 

Potassium    sesgtuoxyplatisulphate,    Pt2O3, 

3SO3,  SO4K2+2H2O. 
(Blondel.) 


Sodium  sesginoxyplatisulphate,  Pt2O3,  3SO3, 

SO4Na2+8H2O. 
Very  sol.  in  H2O.    (Blondel.) 

Oxysulphantimonic  acid. 
See  Sulphoxyantimonic  acid. 

Oxysulpharsenic  acid. 
See  Sulphoxyarsenic  acid. 


Oxysulphazotic  acid, 

/0\ 

(SO3H)3  =  N  -  NO-SO3H. 
Known  only  in  its  salts.     (Glaus,  A.  158. 
52,  194.) 

Has  formula  (SO3H)2N^\N(SO3H)2. 
(Raschig,  A.  241.  161.) 

Potassium  oxysulphazotate,  NO(SO3K)2. 

Insol.  in  alcohol.     (Fremy,  A.  ch.  (3)  15. 
451.) 

According  to  Raschig  the  formula  is 


Very  sol.  in  water,  with  rapid  decomposi- 
tion. (Raschig.) 

See  also  Peroxylaminesulphonate,  potas- 
sium. 

Oxysulphotungstic  acid. 

See  Sulphotungstic  acid. 

Oxysulphovanadic  acid. 

See  Sulphoxyvanadic  acid. 

Ozone,  O3. 

Not  appreciably  sol.  in  H2O.    (Schonbein.) 
Imparts  its  taste  and  properties  to  H2O. 
Williamson.) 

Later,  Carius  (B.  5.  520)  found  that  1000 

vols.  H2O  at  1-2.5°  absorb  5.11  vols.  O3  (red. 

o  0°  and  760  mm.).    He  also  still  later  (A. 

174.  1)  found,  by  conducting  the  gas  for  9-12 

hours   through  H2O,   that    1000  vols,   H2O 

absorb  a  maximum  of  28.160  vols.  O3.    The 

ozonized  oxygen  used  contained  3.44  vols.  Oj 

in  100  vols.  O2.    Since  gases  are  absorbed  in 

roportion  to  their  partial  pressure,  which  is 

rery  small  for  the  O3,  the  amount  of  absorp- 

ion  of  water  for  the  gas  is  very  considerable. 

Carius  calculated  the  coefficient  of  absorption 

it  +1°  to  be  0.834. 

Ozone  is  not  at  all  absorbed  by  H2O;  the 
H2O  through  which  ozone  had  been  passed 
ave  no  reactions  for  ozone.    (Rammelsberg, 
B.  6.  603.) 

Schone  (B.  6.  1224)  corroborates  Carius, 
nd  finds  8.81  vols.  to  1000  vols.  H2O  as  a 
naximum  amount  absorbed. 
Sol.  in  H2O.    (Leeds,  B.  12.  1831.) 


642 


PALLADAMINE  CHLORIDE 


H2O  takes  up  2/3  of  its  vol.  of  O3  at  0°  and 
760  mm.  pressure  and  }/%  of  its  vol.  at  12°, 
or  about  15  times  that  of  oxygen  at  the  same 
pressure  and  temp.  (Mailfert,  C.  R.  1894, 
119.  951.) 

Solubility  in  H2O  at  t°. 


Temp. 

Wt.  Os  dis- 
solved  in  1  1. 
H20 

Wt.  Os  in 
gaseous  mix- 
ture above 
the  solution 

Coefficient 
of  solubility 
of  03 

0 

39.4mgr. 

61  .  5  mgr. 

0.641 

6 

34.3 

61 

0.562 

11.8 

29.9 

59.6 

0.500 

13 

28 

58.1 

0.482 

15 

25.9 

56.8 

0.456 

19 

21 

55.2 

0.381 

27 

13.9 

51.4 

0.270 

32 

7.7 

39.5 

0.195 

40 

4.2 

37.6 

0.112 

47 

2.4 

31.2 

0.077 

55 

0.6 

19.2 

0.031 

60 

0.0 

12.3 

0.000 

(Mailfert,  C.  R.  1894,  119.  952.) 

Solubility  of  ozone  in  acidulated  H^O. 

Coefficient 

Temp. 

of  solubility 

Composition  of  solution 

of  ozone 

30° 

0.240 

] 

33 

0.224 

hi.  H2O+0.7cc.H2SO4 

42.7 

0.174 

J 

49 

0.156 

11.  H2O+0.9cc. 

57 

0.096 

11.     "    +0.3  cc. 

(Mailfert.) 

0.00002  pt.  by  weight  is  sol.  in  1  pt.  by 
weight  H2O  at  ordinary  temp,  and  pressure. 
Ladenburg,  B.  1898,  31.  2510.) 

The  solution  of  O3  in  H2O  cannot  be 
brought  into  equilibrium,  because  when  the 
gas  is  blown  through  the  liquid,  a  portion  is 
continually  decomposed,  although  the  con- 
centration remains  constant.  (Inglis,  Chem. 
Soc.  1903,  83.  1012.) 

About  10  nag.  ozone  are  sol.  in  1  1.  H2O  at 
+2°;  1.5  mg.  ozone  are  sol.  at  +28°.  (Mou- 
fang,  C.  C.  1911,  II.  1674.) 

Solubility  in  0.1-N  H2SO4. 

C  solution:  C  gas =0.23  at  20°;  0.44  at  0°. 
(Luther,  Z.  Elektrochem.  1905,  11.  833.) 

The  absorption  coefficient  of  the  gas  in 
0.1  N  H2SO4  solution  is  0.487.  (Rothmund, 
C.  C.  1912.  I,  1261.) 

Sol.  in  H2C2O4+Aq.    (Jeremin,  B.  11.  988.) 

Completely  absorbed  by  oil  of  turpentine 
and  oil  of  cinnamon.  (Soret,  A.  ch.  (4)  17. 113.) 

Dipalladamine  chloride,  Cl2Pd2(NH3)4Cl4= 


(Deville  and  Debray,  C.  R. 


Palladium,  Pd. 

Not  attacked  by  H2O.  SI.  attacked  by 
HC+Aq,  but  Pd  sponge  or  filings  are  easily 
dissolved  in  warm  HCl+Aq,  with  access  of 
air.  .HNOs+Aq  of  1.2  sp.  gr.  dissolves  Pd 
slightly,  but  it  is  easily  sol.  in  HNO3-f-Aq  of 
1.35  sp.  gr.  (Rose.) 

Easily  sol.  in  aqua  regia.  SI.  sol.  in  cone., 
but  insol.  in  dil.  HI+Aq.  Sol.  in  cone,  boil- 
ing H2SO4.  Sol.  in  boiling  FeCls+Aq.  Sol. 
in  HBr+Aq  with  a  little  HNO3. 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  828. 

Palladium  ammonium  compounds. 

See— 

Dipalladamine  comps.,  Cl2Pd2(NH3)4Cl4. 
Pallado^amine      "       Pd(NH3)4Cl2. 
Palladosamine       "       Pd(NH3)2Cl2. 


SI.  sol.  in  H2O. 
5.  296.) 


Palladium  ^bromide. 
Not  known  in  pure  state. 

Palladium  bromide  with  MBr. 
See  Bromopalladite,  M. 

Palladium  te^rabromide  with  MBr. 
See  Bromopalladate,  M. 

Palladous  phosphorus  bromide,  Pd2P2Bri0. 

Properties  as  the  corresponding  chloride. 
(Strecker,  B.  1909,  42.  1776.) 

Palladium  sw&chloride,  Pd2Cl2. 

Deliquescent.  Decomp.  by  H2O,  NH4C1, 
KI,  or  NH4OH+Aq.  Kane.) 

Sol.  in  acetone.     Naumann,  B.  1904,  37. 

4328.) 

Palladium  ^'chloride,  PdCl2. 

Slowly  but  completely  sol.  in  H2O. 

+2H2O.  Not  deliquescent  when  pure. 
Slowly  sol.  in  H2O.  Much  more  sol.  in  H20 
containing  HC1. 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899,  II. 
1014.) 

Sol.  in  ethyl  acetate.  Naumann,  B.  1904, 
37.  3601.) 

Palladium  bichloride  with  MCI. 
See  Chloropalladite,  M. 

Palladium  tetrachloride  with  MCI. 
See  Chloropalladate,  M. 

Palladous  phosphorus  chloride,  PdCl2,  PC13. 

Decomp.  by  H2O  into  deliquescent  P(OH)S, 
PdCl2.  Decomp.  by  alcohol.  (Fink,  C.  R. 
115.  176.) 

Decomp.  by  H2O.  Sol.  in  CHC13  and  C6H6. 
Insol.  in  ligroin  and  CC14.  (Strecker,  B.  1909, 
42.  1775.) 

PdCl2,  2PC13.  Sol.  in  C6H6,  and  decomp. 
by  HA  (Fink.) 


PALLADOAMINE  CHLORIDE 


643 


Fallacious  chloride  carbon  monoxide,  PdCL, 
2CO. 

Decomp.  by  heat.  (Fink,  C.  R.  1898,  126. 
648.) 

2PdCl2,  SCO.  Decomp.  by  H2O.  Sol.  in 
CC14.  (Fink.) 

Palladium  cfo'fluoride,  PdF2. 

SI.  sol.  in  H2O  or  HF+Aq.  SI.  sol.  while 
moist,  in  NH4OH+Aq;  insol.  after  drying, 
in  NH4OH+Aq.  Insol.  in  boiling  NaF  or 
NaHF2+Aq.  (Berzelius.) 

Palladium  hydride,  Pd2H  (?). 

Palladous  hydroxide,  PdO,  zH2O  (?). 

Easily  sol.  in  acids  or  excess  of  alkali 
hydrates,  and  carbonates +Aq.  Sol.  in  hot 
NH4Cl+Aq.  (Rose.) 

Insol.  in  Na2B4O7,  and  Na2HPO4+Aq. 
(Glaus.) 

Palladic  hydroxide,  PdO2,  zH2O. 

Slowly  sol.  in  acids.  Sol.  in  cone.  HC1+ 
Aq  without  decomp.  With  dil.  HCl+Aq,  C12 
is  evolved.  (Berzelius.) 

Palladous  hydroxide  hydroxylamine, 

Pd(NH3O)4(OH)2. 

SI.  sol.  in  H2O.  Sol.  in  dil.  HC1  and  in  dil. 
H2SO4.  (Zeisel,  A.  1907,  351.  445.) 

Palladous  iodide,  PdI2. 

Insol.  in  H2O.  Can  be  detected  as  a  brown 
coloration  in  presence  of  400,000  pts.  H2O. 
(Lassaigne.) 

SI.  sol.  in  HI+Aq.  Easily  sol.  in  KI+Aq. 
(Lassaigne,  J.  ch.  med.  11.  57.) 

Insol.  in  dil.  HCl+Aq,  but  slightly  sol.  in 
saline  solutions.  (Fresenius.) 

SI.  sol.  in  hot  cone.  HNO3+Aq.  Sol.  in 
H2SO3+Aq,  Cl2+Aq,  Br2+Aq,  I2+Aq,  and 
CN+Aq;  also  in  HCN,  and  MCN+Aq. 
Insol.  in  dil.  H2SO4,  HC1,  H3PO4,  HNO3,  or 
HC2H3O2+Aq,  or  in  the  K,  Na,  or  NH4  salts 
of  those  acids.  Insol.  in  CuCl2,  ZnCl2,  or 
Pb(C2H3O2)2+Aq.  Insol.  in  KBr+Aq  ex- 
cept in  presence  of  a  free  mineral  acid,  but  not 
HC2H3O2.  Insol.  in  sugar  or  starch +Aq, 
uric  acid,  alcohol,  ether,  or  oil  of  lemon. 
Somewhat  sol.  in  urine.  Easily  sol.  in  NH4OH 
+Aq,  even  when  dil.,  with  evolution  of  heat 
and  decomposition.  (Kersten,  A.  87.  28.) 

Insol.  in  alcohol  or  ether. 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Palladous  potassium  iodide. 
See  lodopalladite,  potassium. 

Palladium  sw&oxide,  Pd2O. 

Decomp.  bv  acids  into  palladious  salt  and 
Pd.  (Kane,  Phil.  Trans.  1842,  1.  276.) 

Insol.  in  acids,  even  boiling  aqua  regia. 
(Willm.  B.  26.  220.) 


Palladous  oxide,  PdO. 

Slowly  sol.  in  acids  by  boiling.  (Wohler, 
A.  174.  160.) 

Palladic  oxide,  PdO2. 

Very  si.  attacked  by  acids. 

Palladopalladic  oxide,  4PdO,  PdO2. 

Not  attacked  by  aqua  regia.  (Schneider, 
Pogg.  141.  528.) 

Palladous    oxychloride,    3PdO,    PdCl2+ 

4H20(?). 
Sol.  in  dil.  acids.    (Kane.) 

Palladous  oxychloride  ammonia,  PdO,  PdCl2, 
6NH«(?). 

Sol.  in  HCl+Aq. 

3PdO,  PdCl2,  2NH3+3H20  (?).  Ppt. 
(Kane.) 

Palladium  selenide,  PdSe. 

Insol.  in  HNO3  and  aqua  regia.  (Rossler, 
A.  180.  240.) 

Palladium  sw&sulphide,  Pd2S. 

Not  attacked  by  acids  except  aqua  regia, 
which  attacks  slightly.  (Schneider,  Pogg. 
141.  530.) 

Palladium  monosulphide,  PdS. 

Insol.  in  H2O  or  (NH4)2S+Aq.  Sol.  in 
HCl+Aq.  Pptd.  in  presence  of  10,000  pts. 
H2O.  (Fellenberg,  Pogg.  60.  65.) 

Sol.  in  potassium  thiocarbonate+Aq.  (Ro- 
senbladt,  Z.  anal.  26.  15.) 

A  sol.  colloidal  form  was  obtained  in  very 
dilute  solution.  (Winnsinger,  Bull.  Soc.  (2) 
49.  452.) 

Does  not  exist.  (Kritschenko,  Z.  anorg.  4. 
247.) 

Palladium  bisulphide,  PdS2. 

HNO3  dissolves  out  part  of  the  S.  Easily 
sol.  in  aqua  regia  without  separation  of  S. 
(Schneider.) 

Palladium  sulphide  with  M2S. 
See  Sulphopalladate,  M. 

Palladodiamine  bromide,  Pd(N2H6Br)2. 
Easily  sol.  in  H2O. 

—  bromopalladite,  Pd(N2H6Br)2,  PdBr2. 
Properties  as  the  corresponding  chloropal- 

ladite. 

— —  carbonate. 
Sol.  in  H2O. 

—  chloride,  Pd(N2H6Cl)2. 
Easily  sol.  in  H2O. 


644 


PALLADOAMINE  CHLOROPALLADITE 


Palladocftamine  chloropalladite,  Pd(N2H6Cl)2, 
PdCl2. 

"  Vauquelin's  red  salt."  Insol.  in  cold  H2O. 
(Fischer.) 

Sol.  in  boiling  H2O  with  decomp.  Sol.  in 
HC1  or  HNO3+Aq. 

fluoride. 

Easily  sol.  in  H2O.    (Muller.) 

fluosilicate. 

SI.  sol.  in  cold,  easily  in  warm  H2O.  Insol. 
in  alcohol. 

hydroxide,  Pd(N2H6OH)2. 


Sol.  in  H2O. 

—  iodide,  Pd(N2H6I)2. 
Sol.  in  H2O. 

•  nitrate,  Pd(N2H6NO3)2. 

Easily  sol.  in  H2O,  HNO3,  or  NH4OH+Aq. 
Insol.  in  alcohol. 

palladous  nitrite,  Pd(N2H6NO2)2, 

Pd(NO2)2. 
Easily  sol.  in  H2O. 

—  sulphate,  Pd(N2H6)2SO4+H2O. 
Easily  sol.  in  H2O.    Insol.  in  alcohol. 

sulphite,  Pd(N2H6)2SO3. 

SI.  sol.  in  H2O. 

Palladochloronitrous  acid. 

Potassium  palladochloronitrite, 

Pd(NO2)2Cl2K2. 

Sol.  in  2  pts.  hot,  and  3  pts.  cold  H2O. 
(Vezes,  C.  R.  116.  111.) 

Palladocyanhydric  acid. 

Ammonium  palladocyanide, 

(NH4)2Pd(CN)4  (?). 
Sol.  in  hot  H2O.    (Rossler,  Z.  ch.  1866. 175.) 

Barium ,  BaPd(CN)4+4H2O. 

Not  efflorescent.    Sol.  in  H2O. 

Calcium ,  CaPd(CN)4+4H2O. 

Sol.  in  H2O. 


Cupric 
Ppt. 

Lead- 

Ppt. 


-,  CuPd(CN)4. 


-,  PbPd(CN)4. 


Magnesium ,  MgPd(CN)4. 

Very  sol.  in  H2O. 


Magnesium platinocyanide,  MgPd(CN)jj 

MgPt(CN)4+14H2O. 
Extremely  sol.  in  H2O. 

Potassium ,  K2Pd(CN)4+3H2O. 

Efflorescent.    Sol.  in  H2O. 
+H2O.    Not  efflorescent. 


-,  Ag2Pd(CN)4. 


Silver  - 
Ppt. 


Sodium  — ,  Na2Pd(CN)4. 
Not  efflorescent.    Sol.  in  H2O. 
+H20. 

Palladoiodonitrous  acid. 

Potassium  palladoiodonitrite, 
Pd(NO2)2I2K2+3H2O. 

Effloresces  in  the  air. 

Decomp.  by  H2O  and  dil.  acids.     (Rosen 
heim,  Z.  anorg.  1900,  23.  28.) 

Palladonitrous  acid. 

Potassium    palladonitrite,    K2Pd(NO2)4+ 

2H20. 

Efflorescent;  sol.  in  H2O.    (Lang,  J.  pr.  83 
415.) 

Silver  palladonitrite,  Ag2Pd(NO2)4. 
Easily  sol.  in  hot  H2O.    (Lang.) 


-,  Na2Pd(NO2)4. 


Sodium 

(Fischer.) 

Palladosamine  bromide,  Pd(NH3Br)2. 

Insol.  in  cold,  si.  sol.  in  hot  H2O.  Easih 
sol.  in  HC2H3O2,  H2SO3,  KOH,  NH4OH,  o 
alkali  carbonates +Aq.  (Muller,  A.  86.J341. 

-  carbonate,  Pd(NH3)2CO3. 
Moderately  sol.  in  H2O. 

-  chloride,  Pd(NH3Cl)2. 

Insol.  in  H2O,  but  very  gradually  decomp 
by  boiling  therewith. 

Sol.  in  warm  HC1  or  HNO3+Aq.  Sol.  ii 
cold  NH4OH+Aq.  Sol.  in  KOH+Aq  with 
out  evolution  of  NH3. 

+2H2O.  Efflorescent.  Insol.  in  H20 
(Baubigny,  A.  Suppl.  4.  253.) 

cyanide,  Pd(NH3CN)2. 

Sol.mNH4OH+Aq. 


fluoride. 


Known  only  in  solution. 

hydroxide,  Pd(NH3OH)2. 

Easily  sol.  in  H2O.     Slowly  decomp. 
boiling  with  H2O.    (Muller,  A.  86,  341.) 


PERBORATE,  AMMONIUM 


645 


Palladosamine  iodide,  Pd(NH3I)2. 

Insol.  in  H2O.    Sol.  in  boiling  HNO3  with 
evolution  of  I2.    (Fehling,  A.  39.  106.) 

nitrate. 

Known  only  in  solution,  which  decomp.  on 
evaporation. 

nitrite,  Pd(NH3NO2)2. 

Moderately  sol.  in  H2O.     (Lang.) 

palladous  nitrite,   Pd(NH3NO2)2, 

Pd(N02)2. 

Slowly  sol.   in  cold,    easily  in   hot   H2O. 
(Lang.) 

sulphate,  Pd(NH3)2SO4. 

Moderately  sol.  in  H2O.     (Muller.) 

sulphite,  Pd(NH3)2SO3. 

Easily  sol.  in  H2O.    (Muller.) 

Pentamine  chromium  compounds. 

See— 

Brpmopurpureochromium  compounds. 
Chloropurpureochromium  compounds, 
lodopurpureochromium  compounds. 
Xanthochromium  compounds. 
Roseochromium  compounds. 

Pentamine  cobaltic  compounds. 

See— 

Bromopurpureocobaltic  compounds, 
Chloropurpureocobaltic  compounds. 
Nitratopurpureocobaltic  compounds. 
Nitritocobaltic  compounds, 
Purpureocobaltic  compounds. 
Roseocobaltic  compounds. 
Sulphatopurpureocobaltic  compounds. 
Xanthocobaltic  compounds. 

Pentamine  efo'cobaltic  sulphite. 
See  Roseocobaltic  cobaltic  sulphite. 

Pentamine  iridium  compounds. 

See    Iridoper^amine,    and    Iridoaquopen^- 
amine  compounds. 

Pentamine  rhodium  compounds. 

See— 

Bromopurpureorhodium  compounds. 
Chloropurpureorhodium  compounds, 
lodopurpureorhodium  compounds. 
Nitratopurpureorhodium  compounds. 
Roseorhodium  compounds. 
Xanthorhodium  compounds. 

Pentathionic  acid,  H2S5O6. 

Known  only  in  aqueous  solution. 

Cone,  solution  is  decomp.  by  boiling,  but 
made  stable  by  addition  of  acids. 


Sp.  gr.  of  aqueous  solution  of  pentathionic 
acid  at  22°: 

Sp.gr.  1.233      1.320      1.474      1.506 

%H2S6O6        32.1        41.7        56  59.7 

.(Kessler,  Pogg.  74.  279.) 

Does  not  exist.  (Spring,  Bull.  Acad.  roy. 
Belg.) 

Existence  proven  by  Smith  (Chem.  Soc. 
43.  355.) 

Barium  pentathionate,  BaS5O6+2H2O. 

Easily  sol.  in  H2O.  Aqueous  solution  is 
precipitated  by  alcohol. 

Contains  3H2O.     (Lewes,  C.  N.  43.  41.) 

Barium  pentathionate  tetrathionate,  BaS5O6, 

BaS4O6+6N2O. 

Easily  sol.  in  H2O.  Not  precipitated  from 
aqueous  solution  by  two  vols.  alcohol.  (Lud- 
wig,  Arch.  Pharm.'(2)  61.  264.) 

Cupric  pentathionate,  CuS5O6-f  4H2O. 

Easily  sol.  in  H2O.  (Debus,  Chem.  Soc. 
53.  360.) 

Lead  pentathionate,  PbS5O6+4H2O.       - 
Ppt. 

Potassium  pentathionate,  K2S5O6. 

Sol.  in  H2O.  (Rammelsberg,  J.  B.  1857. 
136.) 

Solution  decomposes  very  quickly  when 
neutral,  but  is  more  stable  in  presence  of  salts 
or  acids. 

Sol.  in  about  2  pts.  H2O. 

Insol.  in  alcohol.  (Debus,  Chem.  Soc.  53. 
295.) 

+H2O.    (Shaw,  Chem.  Soc,  43.  351.) 

+  1^H2O.     (Debus,  A.  244.  76.) 

+2H2O.    (Lewes,  C.  N.  43.  41.) 

Perarsenic  acid. 

Sodium  perarsenate,  NaAsO4. 
(Alvarez,  C.  N.  1906,  94.  270.) 

Perboric  acid. 

Ammonium  perborate,  NH4BO3. 

(Constam  and  Bennett,  Z.  anorg.  1900,  25. 
265.) 

+  ^H2O.  Stable  in  dry  air.  100  pts.  H2O 
at  17.5°  dissolve  1.55  g.  anhydrous  salt. 

Decomp.  in  aqueous  solution  at  ord.  temp. 

Decomp.  by  dil.  and  cone.  H2SO4  and  by 
HC1.  (Melikoff,  B.  1898,  31.  953.) 

+H2O.     (Bruhat,  C.  R.  1905,  140.  508.) 

Much  more  sol.  in  H2O  than  the  Na  salt. 
(Tanatar,  Z.  phys.  Ch.  1898,  26.  133.) 

+3H2O.    (Melikoff,  B.  1898,  31.  954.) 

NH4BO3,  NH4BO4+H2O.  (Petrenko,  C. 
C.  1902, 1.  1192.) 


646 


PERBORATE,  BARIUM 


Barium  perborate,  Ba(BO3)2+7H2O. 

Difficultly  sol.  in  H2O.  (Melikoff,  B.  1898, 
31.  954.) 

Caesium  perborate,  CsBO.3+H2O. 
As  NH4  salt.    (Christensen.) 

Calcium  perborate. 

SI.  sol.  in  H2O.  Decomp.  in  water  much 
more  rapidly  than  the  Ba  salt.  (Melikoff, 
B.  1898,  31.  954.) 

Copper  perborate. 

Very  unstable.  Insol.  in  H2O.  (Melikoff, 
B.  1898,  31.  954.) 

Nickel  perborate. 

Very  unstable.    Insol.  in  H2O.    (Melikoff.) 

Potassium  perborate,  2KBO3+H2O. 

1.25  pts.  are  sol.  in  100  pts.  H2O  at  0°;  2.5 
pts.,  at  15°. 

Insol.  in  alcohol  and  ether.  (Girsewald, 
B.  1909,  42.  867.) 

Potassium    perborate    hydrogen    peroxide, 

2KBO3,  H2O2. 

0.70  pt.  is  sol.  in  100  pts.  H20  at  15°. 
(Girsewald,  B.  1909,  42.  868.) 

Potassium  perc&borate,  KB2O5-f-2H2O. 
Ppt.    (Bruhat,  C.  R.  1905, 140.  508.) 

Rubidium  perborate,  RbBO3+H2O. 

As  Na  salt.    (Christensen.) 

Sodium    perborate,    Na2B4O8+10H2O. 

100  g.  H2O  dissolve  4.2  g.  at  11°;  7.1  g.  at 
22°;  13.8  g.  at  32°.  (Jaubert,  C.  R.  1904, 
134.  796.) 

+4H20.  Slowly  decomp.  in  cold  solution, 
rapidly  when  boiled.  (Tanatar,  Z.  phys.  Ch. 
1898,  26.  132.) 

Sol.  in  H2O.  100  g.  H2O  dissolve  1.17  g. 
Aq.  solution  decomp.  on  warming.  (Melikoff, 
B.  1898,  31.  679.) 

100  g.  H2O  dissolve  2.55  g.  at  15°;  2.69  g. 
at  21°;  2.85  g.  at  26°;  3.78  g.  at  32°.  (Jaubert 
and  Lion,  Rev.  gen.  Chim.  1905.  (7)  8.  163.) 

Uranyl  perborate,  UBO4. 

(Bruhat,  C.  R.  1905,  140.  508.) 

Perbromic  acid,  HBrO4. 

Known  only  in  aqueous  solution,  which  can 
be  concentrated  to  a  thick  liquid  on  water 
bath.  Not  decomp.  by  HC1,  SO2,  or  H2S. 
(Kammerer,  J.  pr.  85.  452;  90.  190.) 

Does  not  exist.  (Muir,  C.  N.  33.  256; 
Maclvor,  C.  N.  33.  35.) 


Barium  perbromate,  Ba(BrO4)2. 

Very  si.  sol.  in  boiling  H2O.     (Kammerer, 
J.  pr.  90.  190.) 

Does  not  exist.    (Wolfram,  A.  198.  95.) 

Potassium  perbromate,  KBrO4. 

Less  sol.  in  H2O  than  KBrO3,  but  more  sol. 
than  KC1O4.     (Kammerer,  J.  pr.  90.  190J 

Does  not  exist.    (Wolfram,  A.  198.  95.) 

Silver  perbromate,  AgBrO4. 

SI.  sol.  in  cold,  more  abundantly  in  hot  H2O. 
(Kammerer,  J.  pr.  90.  190.) 

Does  not  exist.    (Wolfram,  A.  198.  95.) 

Perbromoplatinocyanhydric  acid, 

H2Pt(CN)4Br2+zH2O. 
Deliquescent.    Easily  sol.  in  H2O,  alcohol, 
and  ether.    (Hoist,  Bull.  Soc.  (2)  22.  347.) 

Aluminum  perbromoplatinocyanide, 

Al2[Pt(CN)4Br2]3+22H2O. 
Deliquescent.    Very  sol.  in  H2O. 

Ammonium—,  (NH4)2Pt(CN)4Br2. 
Sol.  in  H2O. 

Barium ,  BaPt(CN)4Br2+5H2O. 

Very  sol.  in  H2O  or  alcohol. 

Cadmium ,  CdPt(CN)4Br2+*H2O. 

Very  sol.  in  H2O. 

Calcium ,  CaPt(CN)4Br2+7H2O. 

Sol.  in  H2O. 

Cobaltous ,  CoPt(CN)4Br2+5H2O. 

Sol.  in  H2O.    SI.  sol.  in  alcohol. 

Glucinum  — ,  GlPt(CN)4Br2. 
Deliquescent.    Sol.  in  H2O. 

Ferrous . 

Very  si.  sol.  in  H2O. 

Lead  — ,  PbPt(CN)4Br2+2H20. 
SI.  sol.  in  H2O. 

Lithium  — — ,  Li2Pt(CN)4Br2. 
Deliquescent.    Sol.  in  H2O. 

Magnesium ,  MgPt(CN)4Br2+zH2O. 

Sol.  in  H2O. 

Nickel ,  NiPt(CN)4Br2+zH2O. 

SI.  sol.  in  H2O.    Sol.  in  NH4OH+Aq. 

Potassium ,  K2Pt(CN)4Br2. 

Sol.  in  H2O. 

+2H2O.    Efflorescent. 


PERCHLORIC  ACID 


647 


Silver  perbromoplatinocyanide, 

Ag2PtBr2(CN)4. 
Ppt.    (Miolati,  Gazz.  ch.  it.  1900,  30.  588.) 

Sodium ,  Na2Pt(ON)4Br2. 

Deliquescent.    Sol.  in  H2O. 

Strontium ,  SrPt(CN)4Br2+7H2O. 

Sol.  in  H20. 

Zinc ,  ZnPt(CN)4Br2+5H2O. 

Not  very  sol.  in  H2O. 


Solution  in  H2O  is  very  stable. 

When  dil.  HClO4+Aq  is  distilled,  H2O  and 
HC1O4  distil  off  until  a  temp,  of  203°  is 
reached,  when  an  acid  of  constant  composi- 
tion containing  71.6-72.2%  HC1O4  (=HC1O4 
+2H2O)  is  obtained.  Forms  hydrate  HC1O4 
-j-H2O,  which  is  deliquescent,  and  dissolves 
in  H2O  with  evolution  of  much  heat.  HC1O4 
is  very  unstable,  HC1O4+H2O  more  stable, 
and  HC1O4+2H2O  is  very  stable.  (Roscoe, 
A.  121.  346.) 


Sp.  gr.  of  HC104+Aq.  at  15°/4°. 


Percarbomc  acid. 

®7 

®7 

O7 

Sp.  gr. 

HC1O4 

Sp.  gr. 

Hdo4 

Sp.  gr. 

/O 

HC1O4 

Ammonium  percarbonate,   (NH4)2CO4+ 
2H2O. 

1.005 

1.00 

1.235 

33.29 

1.465 

54.50 

Sol.  in  H2O  with  evolution  of  NH3.    Insol. 
in  alcohol  and   ether.      (Kasanezky,   C.   C. 
1Q02    T    19fi3  "> 

1.010 
1.015 
1.020 

1.90 

2.77 
3.61 

1.240 
1.245 
1.250 

33.85 
34.40 
34.95 

1.470 
1.475 
1.480 

54.89 
55.18 
55.56 

±U\J&y   JL  .    J.j£UO.y 

1.025 

4.43 

1.255 

35.49 

1.485 

55.95 

1.030 

5.25 

1.260 

36  03 

1.490 

56.32 

Barium  percarbonate,  BaCO4. 

1.035 

6.07 

1.265 

36.56 

1.495 

56.69 

Insol.  in  H2O.     (Merck,  C.  C.  1906,  II. 

1.040 

6.88 

1.270 

37.08 

.500 

57.06 

1743.) 

1.045 

9.68 

1.275 

37.60 

.505 

57.44 

Decomp.  slowly  in  the  air.     Not  rapidly 

1.050 

8.48 

1.280 

38.10 

.510 

57.81 

decomp.  by  H2O.    Rapidly  decomp.  by  acids. 

1.055 

9.28 

1.285 

38.60 

.515 

58.17 

(  Wolff  enstein,  B.  1908,  41.  280.) 

1.060 

10.06 

1.290 

39.10 

.520 

58.54 

1.065 

10.83 

1.295 

39.60 

.525 

58.91 

Potassium  percarbonate,  K2CO4. 
Sol.  in  H2O  with  decomp.     SI.  sol.  in  al- 
cohol,   (v.  Hansen,  Z.  Elektrochem.  1897,  3. 

1.070 
1.075 
1.080 
1.085 

11.58 
12.33 
13.08 
13.83 

1.300 
1.305 
1.310 
1.315 

40.10 
40.59 
41.08 
41.56 

.530 
.535 
.540 
.545 

59.28 
59.66 
60.04 
60.41 

448  ) 
K2C2O6.    Sol.  in  H2O  at  0°  with  only  slight 
decomp.  but  is  decomp.  at  ord.  temp.     SI. 
sol.  in  alcohol.     (Treadwell,  Ch.  Z.  1901,  26. 
inns  "i 

1.090 
1.095 
1.100 
1.105 

14.56 
15.28 
16.00 
16.72 

1.320 
.325 
.330 
.335 

42.03 
42.49 
42.97 
43.43 

.550 
.555 
.560 
.565 

60.78 
61.15 
61.52 
61.89 

±\J\JO.) 

1.110 

17.45 

.340 

43.89 

.570 

62.26 

1  115 

18  16 

345 

44  35 

.575 

62.63 

Rubidium   percarbonate,   Rb2CO4,   2H2O2+ 

1.120 

18.88 

.350 

44.81 

.580 

63.00 

H2O. 

.125 

19.57 

.355 

45.26 

.585 

63.37 

Hydroscopic;  decomp.  by  H2O;  pptd.  by 

.130 

20.26 

.360 

45.71 

.590 

63.74 

alcohol. 

.135 

20.95 

.365 

46.16 

.595 

64.12 

Rb2CO4,  H2O2+2H2O.     Hydroscopic;   de- 

.140 

21.64 

.370 

46.61 

.600 

64.50 

comp.  by  H2O;  pptd.  by  alcohol. 

.145 

22.32 

.375 

47.05 

.605 

64.88 

Rb2CO4+2^H2O.    Hydroscopic;  decomp. 

.150 

22.99 

.380 

47.49 

.610 

65.26 

by  H2O;  pptd.  bv  alcohol.    (Peltner,  B.  1909, 

.155 

23.65 

1.385 

47.93 

.615 

65.63 

42.  1782.) 

.160 

24.30 

1.390 

48.37 

.620 

66.01 

Rb2C2O6.     Very  deliquescent.     (Constam 

1.165 

24.94 

1.395 

48.80 

.625 

66.39 

and  Hansen,  Z.  Elektrochem.  1897,  3.  144.) 

1.170 

25.57 

1.400 

49.23 

.630 

66.76 

1.175 

26.20 

1.405 

49.68 

1.635 

67.13 

Sodium  percarbonate,  Na2CO4+l}/£H2O. 
Sol.  in  H2O  with  gradual  decomp.    (Tana- 
tar,  B.  1899,  32.  1544.) 

1.180 
1.185 
1.190 
1.195 

26.82 
27.44 
28.05 
28.66 

1.410 
1.415 
1.420 
1.425 

50.10 
50.51 
50.91 
51.31 

1.640 
1.645 
1.650 
1.655 

67.51 
67.89 
68.26 
68.64 

1.200 

29.26 

1.430 

51.71 

1.660 

69.02 

Sodium    hydrogen    percarbonate,    4Na2CO4, 

1.205 

29.86 

.435 

52.11 

1.655 

69.40 

H2CO3. 

.210 

30.45 

.440 

52.51 

1.670 

69.77 

Ppt.     (Merck,   Chem.  Soc.   1908,  94.   (2) 

.215 

31.04 

.445 

52.91 

1.675 

70.15 

180.) 

.220 

31.61 

.450 

53.31 

.225 

32.18 

.455 

53.71 

Perchloric  acid,  HC1O4. 

.230 

32.74 

.460 

54.11 

Combines  with  H2O  with  a  hissing  sound 

and  evolution  of  much  heat. 

(Emster,  Z.  anorg.  1907,  62.  278.) 

PERCHLORATES 


Sp.  gr.  of  HCK)t-f  Aq. 


%  HCK>« 

Sp*  gr. 
at  15°  4; 

-V        " 

mt30°4= 

«  50°  4° 

11.14 
35.63 
55.63 
69  SI 

1.0670 

1.2569 
1.4807 
1  6708 

1.2451 

1.4637 

1.0507 
1.2292 
1.4421 
1  62S4 

(Emster,  Z.  anorg.  1907,  62.  279.) 
Sp.  gr.  of  HdO4-rAq. 


and  boOs  at  200*  (Serollas):  has  -1.72-1.S2 

sp.  gr.  and  bofls  at  200°  •  Xativelle,  J.  pr.  26. 

Sol.  in  alcohol  with  decamp.;  often  explo- 
sive. 

+2MHiO.    (v.  Wyck.)    . 
+3H,O.    (T.  Wyek.) 

(v.Wyek.) 


-7     E> 


1 . 767': 
1.7817 

1 


.7386 
.6471 


2901 
1.1778 


y-- 


IHH 

.7259 
.7531 
.7690 
.7756 
.7619 
.7023 
.6110 
.5007 
377- 


1574 


20° 


1.7716 
1.7858 
1.S100 


.7425 
Hi 


am 

2927 
1.1SOO 


.7312 
.7475 
.7751 
.7912 

.7m 

7S40 

.7237 

6311 

SIM 


1  1715 


Sr 

H 


by  wt. 
CtOti* 
tfe 


100 


62 


n  07 

75.59 

H  ^2 

n  AX 

50.51 
39.73 
27.07 


AU  perchkratCB  are  soL  in  HA  KC1O*, 

3\^1\_)^.    J^TWI    C^,  5\_  l\_/4    9QQftCWuftfc   ^fimCPftty* 

They  are  all  deliquescent,  and  sol  in  alcohol, 
excepting  XH^CK)^  KClOt,  Pb(CK)«)^  *»» 
Hg,  C»«K.-  (SerulLis,  A.  ch.  (2)  46,  296.) 


Ahnn 


chl< 


te,  Al 

Very  deliquescent.     (Weinland,  Z. 
1913,  84.  370.) 


sodiom 


ALN  a  dO^)^ 

SL  hygroscopic.  (Wcadand,  Z.  anorg.  1913, 
84.  370. 

SoL  in  acetoaa.  (NaMMon,  B.  19Oi?  37. 
OHL 


(T.  Wyk,  Z, 


of  HC9O4+Aq.  at 


mm  45. 4- 


72.4 

li   v 
65.2 
61.2 
56.65 
•  0 
3S.90 
24  23 
0.0 


_:_;; 


7:  4 
4-0  :: 

6.06 
0.9 


00 


NH  7 
181.2 
162  3 
1^0 
132.4 
114.8 
106.  S 

:  :•:• 


(T.  Wyfc.  Z.  anoKg.  1905, 48. 35.) 
Bpt.  of  BCX>4+Aq.  at   18  mm.  pn 


-.    :  -     "     H  '    .  .  .-  "T 

5-- 

100 

-1     > 

.-•:  1 

>4  S 
79.S 
70.5 

::  :-: 
:-i  - 

-:.r 

70 
9(2 

107 

Permanent.    SoL  in  5  pts.  HjO; 
aoLmafaohoL     MJtorbrrtirii,  Fog. 


300.) 


of  XH<CK)4  in  HsO  at  f. 


G.  per 


0 

8 


100 
107 


115.63 

:••">->•  ±~ 
l  •  :-:• 

--  -,      » 

591.15 


1  MB 

n 
us 

.193 
.21ft 

.221 


(Grin, 


S-.: 


1911.  262.) 


(T.  Wyk,  Z. 


Mi 


I.  36 
(Borne,  A.  1H. 


«O  dboive  1&5 

— *^».«*m 

100  g.  sat,  solution  in  H/)  contain  1.735 
7^5?)  g.  XHdCK)«  a*  l^T.     (Tim  and 
•MMI  Chan.  Soc.  1915^  MT.  36L) 
InaoL  in  cone.  HCK)«+A< 

::•:  r 


PERCHLORATE,  HYDRAZINE 


649 


+3II2O.     Solubility  of  Ba(ClO4)2+3H2O  in 
H20  at  t°. 

Cobaltous  perchlorate,  Co(ClO4),+9H20. 
Solubility  in  H2O  at  t°. 

t° 

G.perlOOg.HjO 

Sp.  gr. 

t° 

G.  anhydrous  salt 
in  100  com. 

Sp.  gr.  of  sat. 
solution  at  t°/4° 

0 

20 
40 

00 

80 
100 
120 
140 

t  r^      i               t  1 

206 
9ft 
308 

432 
497 
.%•! 
645 
758 

1.782 
1.912 
2,009 
2.070 
2.114 
2.155 
2.195 
2.230 

—30.7 
—21.3 
0 
+  7.5 
18 
26 
45 

83.14 
90.57 
100.13 
101.92 
103.80 
113.45 
115.10 

1.5639 
1.5658 
1.5670 
1.5811 
1.5878 

Bismuth  perchlorate,  (BiO)ClO4. 

Insol.  in  IL.O.    Easily  sol.  in  HC1  or  HNO3 

+Aq,  less  c.'isilv  in  ir2SO4+Aq.    (Muir,  C.  N. 
33.  15.) 

Cadmium  perchlorate,  Cd(ClO4)2. 

Very   «l«-li(|iicscciil,.     Sol.  in   H2()  and  al- 
cohol.'   (Sri-alias,  A.  cli.  46.  305.) 

I  III..O.    (Salvadori,  C.  C.  1912,  II.  414.) 

+(>K20.    (S.) 

Cadmium  perchlorate  ammonia,  Cd(CK)4)2, 


Cd(ClO4)2,  4NH8.    (Salvadori,  C.  C.  1912, 
II.  114.) 

Caesium  perchlorate,  CsClO4. 

\  n-y  si.  sol.  in  H2O.    (Rotgers,  Z.  phys.  Ch. 
8.    17.') 

Solubility  in  H,O.     100  g.  H2O  dissolve  at: 
8.5°        14°       33.7°       42°        50° 
O.'.M       1.19       2.99       4.09     5.47  g.  CsClO4, 

60°        70°         84°        99° 
7.30       9.79      16.51     28.57  g.  CsC104. 
(Calzoliiri,  Ace.  Se.  Med.  Ferrara,  1911,  85. 
150.) 

Solubility  in  H2O  at  t°. 


t° 

G.  per  100  g.  H2O 

Sp.  gr. 

5 
25 
80 

0.97 
2.05 
17.05 

1.007 
1.010 
1.084 

(Carlson,  Festsk.  Stockholm,  1911.  262.) 

Calcium  perchlorate,  Ca(ClO4)2. 

Very  deliquescent.  Very  sol.  in  H2O  and 
alcohol.  (Scnillos,  A.  ch.  46.  304.) 

Cerous  perchlorate,  Ce(C104)8+8H2O. 
Very  deliquescent.    (Jolin.) 

Chromic  perchlorate,  Cr(ClO4)3+6H2O. 

Very  hygroscopic.  (Weinland,  Z.  anorg. 
1913,84.  371.) 

+91 U ).  ( '.-in  be  crvst.  from  H2O.  (Wein- 
land.) 


(Golblum  and  Terlikowsky,  Bull.  Soc.  1912, 
(4)  11.  146.) 

+6H2O.  (Salvadori,  Gazz.  ch.  it.  1912, 
42.  (1)  458.) 

Cobalt     perchlorate     ammonia,     Co(ClO4)2 

6NH8. 

Co(ClO4)2,  5NH8. 
Co(ClO4)2,  4NH3,  and  +2H2O. 
Co(ClO4)2,  3NH3,  and  +3H2O. 
Co(ClO4)2,  3NH3+2H2O. 
(Salvadori,  Gazz.  ch.  it.  1912,  42.  (1)  458.) 

Cupric  perchlorate,  basic,  Cu(ClO4)2,  Cu(OH)2. 
Ppt.    (Salvadori,  C.  C.  1912,  II.  414.) 

Cupric  perchlorate,  Cu(ClO4)2. 

Deliquescent.  Sol.  in  H2O  and  alcohol. 
(Serullas,  A.  ch.  46.  306.) 

+4H2O.    (Salvadori,  C.  C.  1912,  II.  414.) 

Cupric  perchlorate  ammonia,  Cu(ClO4)2, 
4NH8+2H2O. 

Not  deliquescent.  Sol.  in  NH4OH+Aq. 
(Roscoe,  A.  121.  346.) 

Cu(ClO4)2,  NH8+H2O. 

Cu(ClO4)2,  2CuO+2H2O,  NH3. 

Cu(ClO4)2,  2CuO+2H2O,  2NH3. 

Cu(ClO4)2,  Cu(OH)2+2H2O,  6NH3. 

Cu(C104)i,  Cu(OH)2+2H20,  4NH3. 

(Salvadori,  C.  C.  1912,  II.  414.) 

Didymium  perchlorate,  Di(ClO4)3+9H2O. 

Very  deliquescent.  Very  sol.  in  H2O  and 
alcohol.  (Cleve.) 

Erbium  perchlorate,  Er(ClO4)3+8H2O. 
Very  deliquescent. 

Glucinum  perchlorate,  G1(C1O4)2+4H2O. 

Very  deliquescent,  and  sol.  in  H2O.  (Atter- 
berg.) 

Hydrazine    perchlorate,     (N2H4)(HC1O4)2  + 

3H2O. 

1  1.  of  sat.  solution  in  H2O  contains  417.2  g. 
at  18°,  sp.  gr.  =  1.264;  669  g.  at  35°,  sp.  gr.  = 
1.391.  (Carlson,  Festsk.  Stockholm,  1911. 
262.) 


650 


PERCHLORATE,  INDIUM 


Indium  perchlorate,  In(ClO4)3+8H2O. 

Deliquescent.  H2O  solution  decomp.  at 
40°  with  separation  of  basic  salt.  Sol.  in 
H2O  and  easily  forms  sat.  solutions.  Sol.  in 
abs.  alcohol,  but  much  less  sol.  in  ether. 
(Mathers,  J.  Am.  Chem.  Soc.  1908,  30.  212.) 

Iodine  perchlorate,  I(C1O4)3+2H2O. 

Decomp.  by  H2O.  Indifferent  toward  or- 
ganic solvents.  (Fichter,  Z.  anorg.  1915,  91. 
135.) 

Iron  (ferrous)  perchlorate,  Fe(C104)2. 

Tolerably  permanent;  sol.  in  H2O.  (Serul- 
las,  A.  ch.  46.  335.) 

Iron  (ferric)  perchlorate,  Fe(ClO4)3. 
Sol.  inH2O.    (Serullas.) 

Iron  (ferric)  sodium  perchlorate, 

[Fe(ClO4)4]Na+6H2O. 
Hydroscopic.     Can  be  cryst.   from  H2O. 
(Weinland,  Z.  anorg.  1913,  84.  366.) 

Lanthanum  perchlorate,  La(ClO4)3+9H2O. 

Extremely  deliquescent.  Sol.  in  H2O  and 
absolute  alcohol.  (Cleve.) 

Lead    perchlorate,    basic,    2PbO,     C12O7  + 


per 
H2O. 


Decomp.  by  H2O  into  an  insol.  more  basic 
salt,  and  sol.  Pb(ClO4)2.    (Marignac.) 

Lead  perchlorate,  Pb(ClO4)2+3H2O. 

Permanent;  extremely  easily  sol.  in  H2O. 
(Roscoe,  A.  121.  356.) 

Sol.  in  about  1  pt.  H2O.    (Serullas.) 

Lithium  perchlorate,  LiClO4. 

Deliquescent.     Sol.  in  H2O   and  alcohol. 
(Serullas.) 

+3H2O.    (Wyrouboff,  Zeit.  Kryst.  10.  626.) 

Magnesium  perchlorate,  Mg(C104)2. 

Deliquescent,  and  sol.  in  H2O  and  alcohol. 
(Serullas.) 

+6H2O.     (Weinland,  Z.  anorg.  1913,  84. 

372.) 


H2O.  Decomp.  by  alcohol.  (Chikashige", 
Chem.  Soc.  1895,  67.  1016.) 

+6H2O.  Very  deliquescent.  (Roscoe,  A. 
121.  356.) 

Permanent.    (Serullas.) 

Mercuric  perchlorate,  basic,  HgO,  2Hg(C104)2. 

Anhydrous.  Ppt.  Insol.  in  either  HC1  or 
HNO3.  Decomp.  and  dissolved  by  a  mixture 
of  the  two.  (Chikashige",  Chem.  Soc.  1905, 
87.  824.) 

+  12H2O.    Very  sol.  in  H2O.    (Chikashige".) 

2HgO,  Hg(C104)2. 

a-salt.  Decomp.  by  H2O.  Sol.  in  acids. 
(Chikashige",  Chem.  Soc.  1895,  67.  1015.) 

/3-salt.  Insol.  in  H2O;  insol.  in  HC1  or 
HNO3.  (Chikashige",  Chem.  Soc.  1905,  87. 
825.) 

Mercuric  perchlorate,  Hg(ClO4)2. 

Very  deliquescent.  Sol.  in  H20;  si.  sol. 
with  decomp.  in  alcohol.  (Serullas,  A.  ch. 
34.  243.) 

+6H2O.  Very  hygroscopic.  Very  sol.  in 
H2O.  Slowly  decomp.  by  H2O,  more  easily 
by  alcohol.  (Chikashige",  Chem.  Soc.  1895, 
67.  1014.) 

Mercuric  perchlorate  bromide,  HgC104Br. 

Decomp.  by  H2O.  (Borelli,  Gazz.  ch.  it. 
1908,  38.  (2)  421.) 

Mercuric    perchlorate    cyanide,    Hg(ClO4)2, 

Hg(CN)2. 
Very  sol.  in  H2O.    Sol.  in  alcohol.    (Borelli.) 

Mercuric  perchlorate  iodide,  Hg(C104)I. 

Deliquescent.  Decomp.  by  H2O.  Sol.  in 
much  alcohol.  Decomp.  by  HNO8.  Com- 
pletely sol.  in  KI  or  KCN-f-Aq.  (Borelli.) 

Mercuric  perchlorate  sulphocyanide, 
Hg(C104)2,  Hg(SCN)2. 

Insol.  in  H2O  and  cone,  acids.  Sol.  in  aqua 
regia.  (Borelli.) 

+6H20.    (Salvadori,  C.  C.  1912,  II.  414.) 

Nickel  perchlorate,  Ni(ClO4)2. 

Deliquescent;  easily  sol.  in  alcohol  and 
H2O.  (Groth,  Pogg.  133.  226.) 


Manganous  perchlorate,  Mn(ClO4)2. 

ouiu.uiiiu.y  111  j.j.2v_/  ai>  u  . 

Very  deliquescent.     Sol.  in  H2O  and  al- 
cohol.    (Serullas,  A.  ch.  46.  335.) 

t° 

G.  anhydrous 
salt  in  100  ccm. 

Sp.  gr.  of  the 
sat.  solution 

+6H2O.  Sol.  in  0.342  pts.H2O.  (Salvadori, 
C.  C.  1912,  II.  414.) 

—30.7 
—21.3 

89.98 

92.48 

Manganous  perchlorate  ammonia,  Mn(ClO4)2, 
5NH3+H2O. 

0 

+7.5 
18 

104.55 
106.76 
110.05 

1.5726 
1.5755 
1  .  5760 

Sol.  in  HC1;  insol.  in  HNO3.     (Salvadori, 

26 

112.15 

1.5841 

C.  C.  1912,  II.  414.) 

45 

118.60 

1  .  5936 

Mercurous  perchlorate,  (HgClO4)2+4H2O. 

(Golblum  and  Terlikowsky,  Bull.  Soc.  1912, 

Very  sol.  in  H2O.    Gradually  decomp.  by 

(4)  11.  147.) 

PERCHLORATE,  POTASSIUM 


651 


-f  5H2O.    (Golblum  and  Terlikowsky.) 
+6H2O.     (Salvador!,  C.  C.  1912,  II.  414.) 
+9H2O.     (Golblum  and  Terlikowsky.) 


Nickel    perchlorate, 

6NH3. 
Ppt.    (Salvadori.) 


ammonia,    Ni(ClO4)2 


Nitrosyl  perchlorate,  NO.O.C1O8+H2O. 

Ppt.;  si.  hydroscopic;  decomp.  by  H2O 
(Hofmann,  B.  1909,  42.  2032.) 

Platinum  perchlorate,  Pt6ClO9+15H2O. 

Insol.  in  H2O.  (Prost,  Bull.  Soc.  (2)  46 
156.) 

Potassium  perchlorate,  KC1O4. 

Sol.  in  57.9  pts.  H2O  at  21.3°  (Longuinine,  A.  121 
123) ;  in  65  pts.  H2O  at  15°  (Serullas,  A.  ch.  (2)  46.  297) ; 
in  88  pts.  H2O  at  10°;  in  55  pts.  H2O  at  100°  (Hutstein, 
J.  B.  1851.  331.) 

Solubility  in  H2O. 

1  pt.  KC1O4  dissolves  in  142.9  pts.  H2O  at 
6°,  and  solution  has  sp.  gr.  =  1.0005;  in  52.5 
pts.  H2O  at  25°,  and  solution  has  sp.  gr.  = 
1.0123;  in  15.5  pts.  H2O  at  50°,  and  solution 
has  sp.  gr,  =  1.0181;  in  5.04  pts.  H2O  at  100°, 
and  solution  has  sp.  gr.  =  1.0660.  (Muir,  C. 
N.  33.  15.) 

1  1.  H2O  dissolves  78.07  millimols.  KC1O4 
at  10°;  120.4  millimols.  at  20°;  179.9  milli- 
mols. at  30°.  (Noyes  and  Sammet,  Z.  phys. 
Ch.  1903,  43.  538.) 

1  1.  H2O  dissolves  0.1475  mol.  KC1O4  at 
25°.  (Rothmund,  Z.  phys.  Ch.  1909,  69.  539.) 

Solubility  in  H2O  at  t°. 


0 
10 
15 
20.5 


G.  KC1O4 

in  100  g. 

H20 


0.70 
1.14 

1.54 
1.90 


50 
70 
99 


G.  KC1O4 

in  100  g. 

H2O 


6.45 
12.3 
22.2 


(Calzolari,  Ace.  Sci.  Med.  Ferrara,  1911,  85. 
150.) 


t° 

G.perlOOg.H2O 

Sp.  gr. 

0 

0.79 

1.007 

20 

1.80 

1.011 

40 

4.81 

1.022 

60 

8.71 

1.033 

80 

14.78 

1.053 

100 

20.98 

1.067 

(Carlson,  Festsk.  Stockholm,  1911.  262.) 

1  1.  H2O  dissolves  0.1481  equivalents 
KC1O4  at  25°.  (Noyes  and  Boggs,  J.  Am. 
Chem.  Soc.  1911,  33.  1652.) 

100  cc.  of  sat.  solution  of  KC1O4  in  H2O  con- 


tains 2.085  g.  KC1O4  at  25.2°.  (Thin  and  Gum- 
ming, Chem.  Soc.  1915,  107.  361.) 

KC1O4  is  sol.  in  22.C  pts.  H2O  at  ord.  temp., 
and  4.00  pts.  at  100°;  in  29.6  pts.  NH4OH  + 
Aq  (cone.)  at  ord.  temp.;  in  30.4  pts.  NH4OH 
+Aq  (1  vol.  cone. +3  vols.  H2O)  at  ord. 
temp.;  in  22.4  pts.  HNO3-j-Aq  (1  vol.  conc.+ 
5  vols.  H2O)  at  ord.  temp.,  and  5.00  pts.  at 
100°;  in  30.4  pts.  HCl+Aq.  (1  vol.  conc.+ 
4  vols.  H2O)  at  ord.  temp.;  45.2  pts.  HC2H302 
+Aq  (1  vol.  commercial  acid-j-1  vol.  H2O) 
at  ord.  temp.;  in  24.4  pts.  NH4C2H3O2+Aq. 
(dil.  HC2H3O2+dil.  NH4OH+Aq)  at  ord. 
temp.,  and  6.00  pts.  at  100°;  in  25.6  pts. 
NH4Cl+Aq  (1  pt.  NH4C1+  10  pts.  H2O)  at 
ord.  temp.,  and  6.00  pts.  at  100°;  in  16.0  pts. 
NH4NO3+Aq  (1  pt.  NH4NO3+10  pts.  H2O) 
at  ord.  temp.,  and  4.00  pts.  at  100°;  in  25.6 
pts.  NaC2H3O2+Aq  (cone.  HC2H3O2  + 
Na2CO3+4  vols.  H2O)  at  ord.  temp.,  and 
7.00  pts.  at  100°;  in  29.2  pts.  Cu(C2H3O2)2  + 
Aq  (Stolba,  Z.  anal.  2.  390)  at  ord.  temp., 
and  7.00  pts.  at  100°;  in  27.2  pts.  cane  sugar 
(1  pt.+lO  pts.  H2O)  at  ord.  temp.;  in  36.8 
pts.  grape  sugar  (1  pt.  +  lO  pts.  H2O)  at  ord. 
temp.  (Approximate.)  (Pearson,  Zeit.  Chem. 
1869.  662.) 

Solubility  of  KC1O4  in  HC104  at  25.2°. 


Normality  of  HC1O< 


0.01 
0.10 
1.00 


1.999 
1.485 
0.527 


(Thin  and  Gumming,  Chem.  Soc.  1915.  107. 
361.) 

Solubility  in  KCl+Aq  at  25°. 


Concentration  of  KC1 
Equivalents  per  litre 


0.04973 
0.09933 


Solubility  of  KCJ04 
Equivalents  per  litre 


0.1282 
0.1123 


(Noves  and  Boggs,  J.  Am.  Chem.  Soc.  1911, 
33.  1652.) 

Solubility  in  K2SO4+Aq  at  25°. 


Concentration  of  K2SC>4 
Equivalents  per  litre 


0.04970 
0.09922 


Solubility  of  KC1O4 
Equivalents  per  litre 


0.1315 
0.1181 


(Noyes  and  Boggs.) 

Very  si.  sol.  in  abs.  alcohol,  and  insol.  if 
alcohol  contains  trace  of  an  acetate.  (Ros- 
coe  )  Insol.  in  alcohol  of  0.835  sp.  gr.  (Schlos- 
ing,  C.  R.  73.  1269.) 

Sol  in  6400  pts.  97.2%  alcohol;  in  5000 
pts.  95.8%  alcohol;  in  2500-3000  pts.  90% 
alcohol;  in  25,000  pts.  alcohol-ether  (2  pts. 
1  pt.  ether).  Practically  insol. 


652 


PERCHLORATE,  POTASSIUM  RUBIDIUM 


in  an  alcoholic  solution  of  HC1O4.     (Wenze' 
Z.  angew.  Ch.  1891.  691.) 

Solubility  of  KC1O4  in  ethyl  alcohol  +Aq  at 
25.2°. 

Solubility  in  H2O  at  t°. 

t°                  G.  in  100  g.  H20 

Sp.  gr. 

0                     1.10 
20                    1.56    - 
40                     3.26 
60                     6.27 
80                   11.04 
100                   15.75 

1.007 
1.010 
1.017 
1.028 
1.050 
1.070 

Vol.  %  alcohol 

soLin^O^aicoho, 

51.2 
93.5 

98.8 

0.754 
0.051 
0.019 

(Carlson,  Festsk.  Stockholm,  1911.  262.) 

Scandium  perchlorate. 
(Crookes,  Roy.  Soc.  Proc.  1908,  80.  A,  518.) 

Silver  perchlorate,  AgClO4. 
Deliquescent.     Sol.   in  H2O   and  alcohol. 
(Serullas,  A.  ch.  46.  307.) 

Sodium  perchlorate,  NaClO4. 
Deliquescent,   and  very  sol.  in  H2O  and 
alcohol.    (Serullas.) 
Not  deliquescent.    (Potilitzin,  J.  russ.  Soc. 
1889,  1.  258.) 

Solubility  in  H2O  at  t°. 

(Thin  and  Gumming,  Chem.  Soc.  1915,  107. 
361.) 

Solubility  in  organic  compds.+Aq.  at  25°. 

Solvent 

Mol.  KC1O4  sol.  in 
1  litre 

0.5-N  methyl  alcohol 
ethyl  alcohol 
propyl  alcohol 
tert.  amyl  alcohol 
acetone 
ether 
glycol 
glycerine 
urea 
ammonia 
diethylamine 
pyridine 
urethane 
formamide 
acetamide 
acetic  acid 
phenol             l 
methylal 
methyl  acetate 

0.1402 
0.1356 
0.1343 
0.1279 
0.1451 
0.1336 
0.1416 
0.1404 
0.1510 
0.1474 
0.1342 
0.1410 
0.1400 
0.1539 
0.1447 
0.1462 
0.1362 
0.1400 
0.1429 

f0                    G.  in  1  1.  of 
solution 

Sp.  gr. 

15                   1076 
50                   1234 
143                   1414 

1.666 
1.731 

1.789 

(Carlson,  Festsk.  Stockholm,  1911.  262.) 
+H2O.    Not  deliquescent.     (Potilitzin.) 

Strontium  perchlorate,  Sr(ClO4)2. 
Very  deliquescent.     Sol.  in  H2O  and  al- 
cohol.   (Serullas,  A.  ch.  46.  304.) 

(Rothmund,  Z.  phys.  Ch.  1909,  69.  539.) 

Insol.  in  methyl  acetate.     (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.     (Naumann, 
B.  1910,  43.  314.) 

Potassium  rubidium  perchlorate, 

KRb2(ClO4)s. 
15.5  g.  are  contained  in  1  1.  solution  sat. 
at  20°;  sp.  gr.  =  1.013.    (Carlson.) 

Rubidium  perchlorate,  RbClO4. 

Sol.  in  92.1  pts.  H2O  at  21.3°.  (Longuinine, 
A.  121.  123.) 

1  pt.  sol.  in  92.1  pts.  H2O  at  21°  as  com- 
pared with  1  pt.  KC1O4  sol.  in  57.9  pts.  H2O 
at  21°.  (Erdmahn,  Arch.  Pharm.  1894,  232. 


Terbium  perchlorate. 

Very  sol.  in  H2O  and  in  alcohol.  (Potratz, 
C.  N.  1905,92.3.) 

Thallous  perchlorate,  T1C1O4. 

1  pt.  salt  dissolves  in  10  pts.  H2O  at  15°, 
and  0.6  pt.  at  100°.  (Roscoe,  Chem.  Soc.  (2) 
4.  504.) 

Solubility  in  H2O  at  t°. 


.6/0.; 

Solubility  in  H2O  at  t°. 

t° 

G.  per  100  g.  H30 

Sp.  gr. 

t° 

G.  RbC104 
in  100  g. 
H20 

t° 

G.  RbClO4 
in  100  g. 
H20 

0 
10 
30 
50 
70 
80 

6.00 
8.04 
19.72     • 
39.62 
65.32 
81.49 

1.060 
1.075 
1.146 
1.251 
1.430 
1.520 

0 

8 
19.8 
30 

2.46 

3.50 

6.28 
9.53 

42.2 
50 

77 
99 

14.94 
19.40 
41.65 
76.5 

(Carlson,  Festsk.  Stockholm,  1911.  262.) 
SI.  sol.  in  alcohol.    (Roscoe.) 

(Calzolari,  Ace.  Sci.  Med.  Ferrara,  1911,  85. 
150.) 

PERCOLUMBATE,  OESIUM 


653 


Thallic  perchlorate,  T1(C1O4)3+6H2O. 

Very  hydroscopic,  sol.  in  H2O.  Decomp. 
in  moist  air.  (Gewecke,  Z.  anorg.  1912,  76. 
274.) 

Uranyl  perchlorate,  (UO2)(C1O4)2+4H2O. 
(Salvadori,  Ch.  Z.  1912,  36.  513.) 
+6H2O.    (Salvadori.) 

Yttrium  perchlorate,  Y(C1O4)3+8H2O. 

Very  deliquescent.    Sol.  in  H2O  and  alcohol. 

(Cleve.) 

Zinc  perchlorate,  Zn(ClO4)2. 

Deliquescent.  Sol.  in  H2O  and  alcohol. 
(Serullas,  A.  ch.  46.  302.) 

+4H2O,  and  6H2O.  (Salvadori,  C.  C. 
1912,  II.  414.) 

Zinc  perchlorate,  ammonia,  Zn(ClO4)2,  4NH3. 
Ppt.    (Salvadori,  C.  C.  1912,  II.  414.) 
Zn(ClO4)2,  6NH3.     (Ephraim,  B.  1915,  48. 

643.) 

Perchromic  acid. 

Sol.  in  ethyl  acetate  and  valerate;  in 
amyl  chloride,  formate,  acetate,  butyrate, 
and  valerate.  (All  give  blue  solutions.) 

Insol.  in  CS2,  C6H6,  CHC13,  CC14,  C6H5NH2, 
C6H5NO2  and  toluene.  (Grosvenor,  J.  Am. 
Chem.  Soc.  1895,  17.  41-43.) 

H3CrO8+2H2O.  Decomp.  above  —30°. 
(Riesenfeld,  B.  1914,  47.  552.) 

Ammonium  perchromate,  (NH4)3CrO8. 

Very  unstable.  SI.  sol.  in  cold  H2O.  De- 
comp. by  cone.  H2SO4.  Insol.  in  pure  al- 
cohol and  pure  ether.  Decomp.  by  boiling 
alcohol  containing  more  than  50%  H2O. 
(Wohlers,  B.  1905,  38.  1888.) 

CrO4,  3NH3.  Sol.  in  10%  NH4OH+Aq; 
sol.  in  H2O  with  decomp.,  insol.  in  other 
solvents.  (Wiede,  B.  1897,  30.  2181.) 

NH4CrO6,  H2O2.  Decomp.  in  the  air. 
Sol.  in  ice  cold  H2O,  decomp.  when  warmed. 
Insol.  in  alcohol,  ether,  ligroin  and  CHC13. 
(Wiede,  B.  1898,  31.  518.) 

Ammonium    hydrogen     perchromate, 

Cr02(O.O.NH4)(O.OH). 
Sol.  in  H2O  with  decomp.    Difficultly  sol. 
in  cold  abs.  alcohol.    (Hofmann,  B.  1904,  37. 
3406.) 

Barium  perchromate,  BaCr2O8. 

(Byers  and  Reid,  Am.  Ch.  J.  1904,  32.  513.) 

Calcium  perchromate,  CaCr2O8. 

Very  sol.  in  H2O.  (Mylius,  B.  1900,  33. 
3689;  Byers  and  Reid,  Am.  Ch.  J.  1904,  32. 
513.) 

Lithium  perchromate,  Li2Cr2O8. 

(Byers  and  Reid,  Am.  Ch.  J.  1904,  32.  511.) 


Magnesium  perchromate,  MgCr2O8. 
(Byers  and  Reid.) 

Potassium  perchromate,  K3CrO8. 

SI.  sol.  in  cold  H2O.  Decomp.  by  cone. 
H2SO4.  Insol.  in  pure  alcohol  and  pure 
ether.  Decomp.  by  boiling  alcohol  contain- 
ing more  than  50%  H2O.  ( Wohlers,  B.  1905, 
38.  1888.) 

+xH2O.  Sol.  in  H2O  at  0°  without  de- 
comp. (Riesenfeld  and  Kutsch,  B.  1908,  41. 
3948.) 

K2Cr2O8.  Sol.  in  H2O.  Decomp.  in  the 
air.  (Byers  and  Reid,  Am.  Ch.  J.  1904,  32. 
505.) 

KCrO6,  H2O2  or  KH2CrO7.  Sol.  in  ice  cold 
H2O,  decomp.  when  warmed;  explosive. 
(Wiede,  B.  1898,  31.  520.) 

Sodium  perchromate,  Na3CrOs. 

SI.  sol.  in  cold  H2O.  Decomp.  by  cone. 
H2SO4.  Insol.  in  pure  alcohol  and  pure  ether. 
Decomp.  by  boiling  with  ale.  containing  more 
than  50%  H2O.  (Wohlers,  B.  1905,  38.  1888.) 

NafiCf2O16+28H2O.  Efflorescent.  SI.  sol. 
in  cold,  easily  in  hot  H2O,  with  decomp. 
Not  decomp.  by  NaOH  +Aq.  (Haussermann, 
J.  pr.  (2)  48.  70.) 

Na2Cr2O8.  (Byers  and  Reid,  Am.  Ch.  J. 
1904,  32.  511.) 

Perchloroplatinocyanhydric  acid, 

H2Pt(CN)4Cl2+4H2O. 
Very  sol.  in  H2O  and  alcohol. 

Ammonium  perchloroplatinocyanide, 

(NH4)2Pt(CN)4Cl2+2H2O. 
Sol.  in  H2O. 

Barium ,  BaPt(CN)4Cl2+5H2O. 

Very  sol.  in  H2O. 

Calcium ,  CaPt(CN)4Cl2. 

Sol.  in  H20. 


Magnesium  — 
Sol.  in  H2O. 


-,  MgPt(CN)4Cl2+zH20. 


Manganous ,  MnPt(CN)4Cl2+5H2O. 

Sol.  in  H2O  and  alcohol. 

Potassium ,  K2Pt(CN)4Cl2+2H2O. 

Very   efflorescent,    and   sol.   in   H20    and 
alcohol. 

Percolumbic  acid,  HCbO4+nH2O. 

Insol.  in  H2O.    Sol.  with  decomp.  in  warm 
H2SO4.    (Melikoff,  Z.  anorg.  1899,  20.  341.) 

Caesium  percolumbate,  Cs3CbO8. 

Ppt.     (E.  F.  Smith,  J.  Am.  Chem.  Soc. 
1908,  30.  1658.) 


654 


PERCOLUMBATE,  CAESIUM  MAGNESIUM 


Caesium  magnesium  percolumbate, 

MgCsCbO8+8H2O. 

Sol.  in  H2O  without  decomp.  (E.  F. 
Smith.) 

Calcium  potassium  percolumbate, 

CaKCbO8+4H2O. 
Difficultly  sol.  in  H2O.    (E.  F.  Smith.) 

Calcium  sodium  percolumbate,CaNaCbO8  + 

4H20. 
Difficultly  sol.  in  H2O.    (E.  F.  Smith.) 

Magnesium  potassium  percolumbate, 

MgKCbO8+7H2O. 

Sol.  in  H2O  without  decomp.  (E.  F. 
Smith.) 

Magnesium  rubidium  percolumbate, 

MgRbCbO8+7^H2O. 
Sol.  in  H2O  without  decomp.    (E.  F.  Smith.) 

Magnesium  sodium  percolumbate, 

MgNaCbO8+8H2O. 
Sol.  in  H2O  without  decomp.    (E.  F.  Smith.) 

Potassium  percolumbate,  K3CbO8. 

Sol.  in  H2O.  Ppt.  from  aq.  solution  by 
alcohol.  (E.  F.  Smith.) 

K4Cb2On+3H2O.  Sol.  with  decomp.  in 
H2O.  Ppt.  by  alcohol.  Sol.  in  KOH+H2O2 
+Aq.  (Melikoff,  Z.  anorg.  1899,  20.  342.) 

Rubidium  percolumbate,  Rb3Cb08. 

Sol.  in  H2O.  '  Insol.  in  alcohol.  (E.  F. 
Smith.) 

Sodium  percolumbate,  Na3CbO8. 

Sol.  "in  H2O.  Insol.  in  alcohol.  (E.  F. 
Smith.) 

Perf erricyanhydric  acid. 

Potassium     perferricyanide,     K2Fe(CN)6+ 

H20  (?). 

Very  hygroscopic,  and  sol.  in  H20.  Nearly 
insol.  in  absolute  alcohol.  Decomp.  by  hot 
H2O.  (Skraup,  A.  189.  368.) 

Periodic  acid,  HBIO6. 

Deliquescent  in  moist  air;  very  sol.  in  H2O. 
(Bengieser,  A.  17.  254.) 

Rather  easily  sol.  in  alcohol  and  Aether. 
(Bengieser.) 

Rather  easily  sol.  in  alcohol,  less  in  ether. 
(Langtoch.) 

SI.  sol.  in  alcohol,  still  less  in  ether.    (Lang- 
lois,  J.  pr.  66.  36.) 
Sp.  gr.  of  H5IO6+Aq. 

H5IO6+  20H2O  =  1.4008. 
H5IO6+  40H20  =  1.2165. 
H5IO6  +  80H2O  =  1.1121. 
H5IO6  +  160H2O  =  1.0570. 
H6IO6+320H2O  =  1.0288. 
(Thomsen,  B.  7.  71.) 


Periodates. 

Most  periodates  are  insol.  or  si.  sol.  in  H2O; 
all  are  insol.  or  very  si.  sol.  in  alcohol,  but 
they  all  dissolve  in  dil.  HNO3+Aq.  (Ben- 
gieser.) 

Aluminum  wetoperiodate,  A1(IO4)3+3H2O. 

Stable  in  solution  containing  HNO3. 
(Eakle,  C.  C.  1896.  II,  649.) 

Ammonium  metoperiodate,  NH4IO4. 

SI.  sol.  in  HoO.  Cryst.  with  3H2O  (Ihre,  B. 
3.  316),  2H2O  (Langlois,  A.  ch.  (3)  34.  257). 

Stable  in  solution  containing  free  ammonia. 
(Eakle,  Zeit.  Kryst.  1896,  26.  258-88.) 

100  pts.  H2O  dissolve  2.7  pts.  NHJO4  at 
16°;  sp.  gr.  of  sat.  solution  at  16°/4°  =  1.0178. 
(Barker,  Chem.  Soc.  1908,  93.  17.) 

Ammonium  dzmesoperiodate,  (NH4)4I2Og  + 
3H2O. 

Sol.  in  H2O.  (Rammelsberg,  Pogg.  134. 
379.) 

Stable  in  solution  containing  free  ammonia. 

Two  modifications.  (Eakle,  Zeit.  Kryst. 
1896,  26.  558-88;  C.  C.  1896.  II,  649.) 

Ammonium  lithium  dimesoperiodate, 

(NH4)2Li2I209+7H20. 
Sol.  in  H2O.    (Ihre.) 

Ammonium  magnesium  mesoperiodate, 

NH4MgIO5+3H2O. 

Precipitate.  (Rammelsberg,  Pogg.  134. 
510.) 

Barium  metoperiodate,  Ba(IO4)2. 
Known  only  in  solution. 

Barium  dmesoperiodate,  Ba2I2O9. 

SI.  sol.  in  H2O;  easily  sol.  in  dil.  HNO3+ 
Aq.  (Rammelsberg,  Pogg.  134.  391.) 

Cryst.  also  with  3H2O,  5H2O,  and  7H2O. 

Barium  mesoperiodate,  Bas(IO5)2+6H2O. 
(Ihre.) 

Barium  or^operiodate,  Ba5(IO6)2. 

Insol.  in  H2O.  Sol.  in  HNO3+Aq.  (Ram- 
melsberg.) 

Barium  dimesodiperiodate,  Ba5I4Oi9+5H2O. 

Precipitate.  Sol.  in  dil.  HNO3+Aq. 
(Rammelsberg,  Pogg.  134.  395.) 

Barium  periodate  tungstate. 
See  Tungstoperiodate,  barium. 

Caesium  metoperiodate,  CsIO4. 

SI,  sol.  in  cold  H2O;  readily  sol.  in  hot  H2O. 
(Wells,  Am.  Ch.  J.  1901,  26.  279.) 

2.15  pts.  are  sol.  in  100  pts.  H2O  at  15°. 
Sp.  gr.  of  the  sat.  aq.  solution  at  15°/4°  = 
1.0166.  (Barker,  Chem.  Soc.  1908,  93.  17.) 


PERIODATE,  MAGNESIUM 


655 


Caesium  periodate  hydrogen  fluoride,  2CsIO4, 

3HF+H2O. 

Sol.  in  40-60%  HF+Aq.  Decomp.  by 
H2O.  Efflorescent.  (Wemland,  Z.  anorg. 
1899,  22.  263.) 

Cadmium  raetaperiodate,  Cd(IO4)2. 
Ppt.    (Rammelsberg,  Pogg.  134.  516.) 

Cadmium  cforaesoperiodate,  Cd2I2O9+9H2O. 
Insol.  in  H2O.    (Rammelsberg.) 

Cadmium  raesoperiodate,  Cd3(IO5)2+5H2O. 

Ppt. 

CdHIO5.    (Kimmins,  Chem.  Soc.  66.  151.) 

Cadmium  t&periodate,  Cd4l2On+3H2O. 
Insol.  in  H2O.    (Rammelsberg.) 


Cadmium  periodate, 

Insol.  in  H2O.    (Rammelsberg.) 

Calcium  wetaperiodate,  Ca(IO4)2. 

Sol.  in  H5IO6+Aq  and  acids.  (Rammels- 
berg, Pogg.  134.  405.) 

Calcium    dmesoperiodate,    Ca2I2O9+7H2O, 

and  9H2O. 

SI.  sol.  in  H2O.    (Rammelsberg.) 
+3H2O.    (Langlois.) 

Calcium  orthoperiodsite,  Ca5(IO6)2. 

Insol.  in  H2O.  Sol.  in  HNO3+Aq.  (Ram- 
melsberg, Pogg.  44.  577.) 

Cobaltous  periodate,  7CoO,  2I2O7-|-18H2O. 

Attacked  by  HC1,  and  sol.  on  warming. 
Slowly  but  completely  sol.  in  NHO3.  (Lautsch, 
J.  pr.  100.  89.) 

Could  not  be  obtained  by  Rammelsberg. 

Cupric  cforaesoperiodate,  Cu2I2O9+6H2O. 

Decomp.  by  H2O  without  dissolving. 
(Rammelsberg.) 

Cupric  ort/ioperiodate,  Cu2HIO6. 

Very  sol.  in  HNO3  +Aq.  (Kimmins,  Chem. 
Soc.  55.  150.) 

Cupric  cfo'periodate,  Cu4I2On+H2O. 

Insol.    in   H2O;    sol.    in   dil.    HNO3+Aq. 

(Rammelsberg.) 
+7H2O.    (R.) 

Cupric  periodate,  5CuO,  I2O6+5H2O. 
Wholly  insol.  in  H2O.     (Rammelsberg,  B. 

1.73.) 

Didymium  peroidate,  Di2O2(IO4)2. 

Precipitate. 

DiIO5+4H2O.  Ppt.  (Cleve,  Bull.  Soc.  (2) 
43.  362.) 


Erbium  periodate. 

Sol.  inH2O.    (Hoglund.) 

Glucinum  periodate,  G13(IO5)2+11H2O. 

Decomp.  by  H2O  without  dissolving.  Eas- 
ily sol.  in  HNO3+Aq. 

+13H2O.  Nearly  insol.  in  H2O.  (Atter- 
berg,  B.  7.  474.) 

Iron  (ferrous)  orZ/ioperiodate,  Fe6(IO6)2. 
(Kimmins,  Chem.  Soc.  55.  150.) 
FeH3IO6.    (Kimmins.) 

Iron  (ferric)  periodate,  2Fe2O3,  I2O7+21H2O. 
Ppt.    (Rammelsberg.) 

Iron  (ferric)  dmesoperiodate,  FeHI2O9. 

Insol.  in  dil.  HNO3+Aq.  (Kimmins, 
Chem.  Soc.  55.  149.) 

Iron  (ferric)  wetaperiodate,  Fe(IO4)3. 
(Kimmins.) 

Lanthanum  periodate,  La(IO4)3+2H2O. 

Precipitate.    (Cleve.) 

Lead  wetaperiodate,  Pb(IO4)2. 
Sol.  in  HNO3+Aq.    (Kimmins.) 

Lead  or^operiodate,  Pb3H4(IO6)2. 

Sol.  in  HN03+Aq.  (Kimmins,  Chem.  Soc. 
55.  149.) 

Lead  mesoperiodate,  Pb3(IO6)2+2H2O. 

Insol.  in  H2O  or  excess  of  periodic  acid+ 
Aq.  Decomp.  by  dil.  H2SO4+Aq.  (Ben- 
gieser,  A.  17.  254.) 

Lithium  wetoperiodate,  LiIO4. 

Difficultly  sol.  in  H2O.  (Rammelsberg,  B. 
1.  132.) 

Somewhat  deliquescent. 

+H2O;  sol.  in  H2O.  (Barker,  Chem.  Soc. 
1911,  99.  1326.) 

Lithium  dmesoperiodate,  Li4I2O9+3H2O. 

Very  si.  sol.  in  H2O.  (Rammelsberg,  Pogg. 
134.  387.) 

Lithium  ortftoperiodate,  Li5IO6. 

H2O  dissolves  out  a  slight  amount  of  Lil. 
Easily  sol.  in  HNO3+Aq.  (Rammelsberg, 
Pogg.  137.  313.) 

Magnesium  wetoperiodate,   Mg(IO4)2-f 

10H2O. 
Easily  sol.  in  H2O.    (Rammelsberg.) 

Magnesium  diperiodate,  Mg4I2Ou+6H2O,  or 

9H2O. 

SI.  efflorescent.  Insol.  in  H2O.  (Rammels- 
berg.) 


656 


PERIODATE,  MAGNESIUM 


Magnesium  cftmesoperiodate,  Mg2I2O9  + 

3H2O. 

(Rammelsberg,  Pogg.  134.  499.) 
+  15H2O.    Insol.  in  H2O.    Sol.  in  periodic 

acid-f-Aq.    (Langlois.) 

Manganic  periodate. 
See  Manganiperiodic  acid. 

Mercurous    cfoperiodate,    5Hg2O,     I2O7,     or 

4Hg2O,  I2O7  =  Hg8I2On. 
Insol.  in  H2O.     Easily  sol.  in  HNO3+Aq 
and  in  HCl+Aq.    (Lautsch,  J.  pr.  100.  86.) 

Mercuric  or^operiodate,  Hg6(IO6)2. 

Insol.  in  H2O.  Easily  sol.  in  HC1.  SI.  sol. 
in  HNO3.  (Lautsch.) 

Mercuric  potassium  periodate,  lOHgO,  5K2O, 

6I207. 

Insol.  in  H2O.  Difficultly  sol.  in  warm 
HNOs  without  decomp.  (Rammelsberg, 
Pogg.  134.  526.) 

Nickel  c&mesoperiodate,  Ni2I2O9. 
(Kimmins,  Chem.  Soc.  56.  151.) 

Nickel  mesoperiodate,  Ni3(IO5)2. 
(Kimmins.) 

Nickel  periodate,  7NiO,  4I2O7+63H2O. 

Insol.  in  H2O.  Easily  sol.  in  H5IOe+Aq. 
(Rammelsberg,  Pogg.  134.  514.) 

Potassium  metaperiodate,  KIO4. 

SI.  sol.  in  H2O.  Sol.  in  290  pts.  cold  H2O. 
(Rammelsberg,  Pogg.  134.  320.) 

Almost  insol.  in  KOH+Aq. 

0.66  pt.  is  sol.  in  100  pts.  H2O  at  13°.  Sp. 
gr.  of  the  sat.  sol.  at  13°/4°  =  1.0051.  (Barker, 
Chem.  Soc.  1908,  93.  16.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,42.3790.) 

Potassium  mesoperiodate,  K3IO6+4H2O. 
Deliquescent.    Easily  sol.  in  H20.     (Ihre.) 

Potassium  c&mesoperiodate,  K4I2O9+9H2O. 

Sol.  in  9.7  pts.  cold  H2O.  (Rammelsberg, 
Pogg.  134.  320.) 

Sol.  in  KOH+Aq. 

+3H2O. 

Potassium  hydrogen  dimesoperiodate, 

K3HI2O9. 

Less  sol.  in  H2O  than  KIO4.  (Kimmins, 
Chem.  Soc.  51.  356.) 

Potassium  manganic  periodate. 
See  Manganiperiodate,  potassium. 

Potassium  zinc  periodate,  K2O,  4ZnO,  2I2O7 

+4H20. 
Ppt.    (Rammelsberg,  Pogg.  134.  368.) 


Potassium  periodate  tungstate. 
See  Tungstoperiodate,  potassium. 

Rubidium  periodate,  RbIO4. 

0.65  pt.  is  sol.  in  100  pts.  H2O  at  13°.  Sp. 
gr.  of  the  sat.  aq.  solution- at  13°/4°  =  1.0052. 
(Barker,  Chem.  Soc.  1908,  93.  16.) 

Samarium  periodate,  Sm(IOj+4H2O. 
Precipitate.    (Cleve.) 

Silver  metaperiodate,  AgIO4. 

Decomp.  by  cold  H2O  into  Ag4I2O9+3H2O, 
and  by  warm  H2O  into  Ag4I2O9-}-H2O.  (Am- 
mermiiller  and  Magnus,  Pogg.  28.  516.) 

+H2O.    Insol.  ppt.    (Kimmins.) 

Silver  mesoperiodate,  Ag3IO5. 

(Fernlunds,  J.  pr.  100.  99.) 

Ag2HIO5.  Insol.  ppt.  (Kimmins,  Chem. 
Soc.  51.  358.) 

Ppt.  by  dil.  HNO3;  sol.  in  HNO3.  (Rosen- 
heim,  A.  1899,  308.  57.) 

Silver  cfomesoperiodate,  Ag4I2O9+H2O,  or 
3H2O. 

Insol.  ppt.    (Kimmins.) 

Decomp.  by  boiling  H2O  into  Ag6IO6. 
(Rammelsberg.) 

Silver  ori/ioperiodate,  Ag5IO6. 

Sol.  inHNO3orNH4OH-fAq.  (Rammels- 
berg, Pogg.  134.  386.) 

Sol.  in  excess  NH4OH+Aq;  pptd.  by 
HNO3.  (Rosenheim,  A.  1899,  308.  56.) 

Ag3H2IOe.  Insol.  ppt.  (Kimmins,  Chem. 
Soc.  51.  358.) 

Ag2H3IO6.    As  above.    (Kimmins.) 
•   Sol.  in  dil.  HNO3.     (Rosenheim,  A.  1899, 
308.  53.) 

Silver  eftperiodate,  Ag8I2On. 

SI.  sol.  in  HNO3+Aq;  insol.  in  NH4OH+ 
Aq.  (Lautsch,  J.  pr.  100.  75.) 

Silver  cfo'wesocfo'periodate,  Agi0I4Oi9. 

HNO3+Aq  dissolves  out  Ag2O.  Insol.  in 
NH4OH+Aq.  (Lautsch.) 

Sodium  metoperiodate,  NaIO4. 

Easily  sol.  in  H2O. 

+2H2O.    (Langlois.) 

+3H2O.  Efflorescent;  sol.  in  12  pts.  H2O 
at  ord.  temp.  (Rammelsberg,  J.  pr.  103.  278.) 

Sodium  ^mesoperiodate,  Na4I2O9+3H2O. 

Scarcely  sol.  in  cold,  si.  sol.  in  hot  H2O. 
(Magnus  and  Ammermiiller,  Pogg.  28.  514.) 

Very  sol.  in  dil.  HNOs+Aq.    (Langlois.) 

Sol.  in  HC2H3O2+Aq  with  decomp. 
(Bengieser,  A.  17.  254.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790,) 

+4H20. 


PERMANGANATE,  CUPRIC 


657 


Sodium  raesoperiodate,  Na3IO6+5/4H2O. 

Sol.  in  H2O.    (Ihre.) 

-f  H2O  =  Na3H3IO6.  Less  sol.  in  H2O  than 
Na4I2O9  +  3H2O(  =  Na2H3IO6).  (Kimmins, 
Chem.  Soc.  61.  357.) 

Sodium  orf/ioperiodate,  Na5IO6. 

Na2H3IOc.  Correct  composition  for 
Na4I2O9+3H2O.  (Kimmins.) 

Na3H2IOe.  Correct  composition  for  Na3IOs 
+H2O.  (Kimmins.) 

Strontium  metaperiodate,  Sr(IO4)2+6H2O. 
Sol.  in  H2O. 

Strontium  cfowesoperiodate,  Sr2I2Og. 
Decomp.  by  H2O. 
+3H2O. 

Strontium  raesoperiodate,  Sr3(IO5)2. 
Precipitate. 


Strontium  or^/ioperiodate, 

(Rammelsberg,  Pogg.  44.  577.) 

Thallic  periodate,  3T12O3,  I2O7+30H2O. 

Insol.    in    H2O.      Decomp.    by    alkalies. 
(Rammelsberg,  B.  3.  361.) 

Thorium  periodate. 

Precipitate.    Sol.  in  HNO3+Aq. 

Uranous  periodate. 

Precipitate,  which  quickly  decomposes. 

Ytterbium  periodate,  YbIO5+2H2O. 

Hydroscopic.     (Cleve,  Z.  anorg.  1902,  32. 
136.) 

Yttrium  periodate,  Y2(IO6)2+8H2O. 

Very  slightly  sol.    (Cleve.) 

3Y2O3,  2I2O7+6H2O.  Precipitate.  (Cleve.) 

Zinc  dimesoperiodate,  Zn2I2O9+6H2O. 
(Rammelsberg,  Pogg.  134.  513.) 

Zinc  periodate,  3ZnO,  2I2O7+7H2O. 

(Langlois.) 

Zinc  ^'periodate,  Zn4I2On+H2O. 

Easily  sol.  in  H2O,  si.  acid  with  HNO3. 
(Langlois,  A.  ch.  (3)  34.  257.) 


Zinc  dimesodiperiodaie, 
(Rammelsberg.) 


(?). 


Zinc  periodate,  9ZnO,  2I2O7  +  12H2O. 
(Rammelsberg.) 

Periodoplatinocyanhydric  acid. 

Barium  periodoplatinocyanide,  BaPt(CN)j2 

+rcH2O. 

Easily  sol.  in  H2O  or  alcohol.    (Hoist,  Bull. 
Soc.  (2)  22.  347.) 


Potassium  periodoplatinocyanide, 
K2Pt(CN)J2. 

Permanent.    Easily  sol.  in  H2O  or  alcohol. 

Permanganic  acid,  HMnC>4. 

Known  only  in  solution,  which  decomposes 
by  evaporation  or  warming. 

Permanganates. 

All  permanganates  are  sol.  in  H2O,  except- 
ing AgMnO4,  which  is  si.  sol. 

Ammonium  permanganate,  NH4Mn04. 
Sol.  in  12.6  pts.  H2O  at  15°.    (Aschoff.) 
Sol.  in  H2O  with  decomp.     (Christensen, 

Z.  anorg.  1900,  24.  206.) 

Barium  permanganate,  Ba(MnO4)2. 
Sol.  in  H2O. 

Cadmium  permanganate,  Cd(MnO4)2+8H2O. 
Stable.    (Klobb,  Bull.  Soc.   1894,    (3)   11 
607.) 

Cadmium  permanganate  'ammonia, 

Cd(MnO4)2,  4NH3. 

Sol.  in  HoO  with  decomp.     (Klobb,  Bull. 
Soc.  (3)  3.  510.) 

Caesium  permanganate,  CsMnO4. 

SI.  sol.  in  cold,  somewhat  more  easily  sol. 
in  hot  H2O.    (Muthmann,  B.  1893,  26.  1018.) 

Solubility  in  H2O. 

100  ccm.  of  the  sat.  solution  contain  at: 

1°  19°  59° 

0.097        0.23          1.25  g.  CsMnO4. 

(Patterson,   J.   Am.   Chem.    Soc.    1906,   28. 
1735.) 

Calcium  permanganate,  Ca(MnO4)2+5H2O. 
Deliquescent. 

Cupric  permanganate. 
Deliquescent. 


658                                PERMANGANATE  AMMONIA,  CUPRIC 

Cupric  permanganate  ammonia,  Cu(MnO4)2, 
Sol.  in  H2O  with  slow  decomp.     (Klobb, 

Solubility  in  H2O  at  t°. 
p  =  pts.  KMnO4  sol.  in  100  pts.  H2O  at  t°. 

Bull.  Soc.  (3)  3.  509.) 

t° 

P 

t° 

p 

t° 

p 

t° 

P 

Didymium    permanganate,    Di(MnO4)3  + 

0 
1 

2.76 
2.90 

19 
20 

6.26 
6.48 

38- 
39 

11.74 
12.12 

57 

58 

20.29 
20.83 

21H2O. 

2 

3.06 

21 

6.70 

40 

12.51 

59 

21.39 

SI.  sol.  in  H2O.     (Frerichs  and  Smith,  A. 

3 

3.22 

22 

6.94 

41 

12.91 

60 

21.96 

191.  331.) 

4 

3.38 

23 

7.18 

42 

13.31 

61 

22.55 

Has  not  been  prepared.    (Cleve,  B.  11.  912.) 

5 

3.54 

24 

7.42 

43 

13.72 

62 

23.15 

6 

3.70 

25 

7.68 

44 

14.14 

63 

23.76 

Lanthanum     permanganate,      La(MnO4)3+ 

7 
8 

3.86 
4.04 

26 

27 

7.94 
8.20 

45 
46 

14.56 
15.00 

64 
65 

24.38 
25.01 

Ppt.    (Frerichs  and  Smith,  A.  191.  331.) 
Has  not  been  prepared.    (Cleve,  B.  11.  910.) 

9 
10 
11 

4.22 
4.40 
4.58 

28 
29 
30 

8.48 
8.77 
9.07 

47 
48 
49 

15.44 

15.88 
16.32 

66 
67 

68 

25.67 
26.34 
27.03 

12 

4.78 

31 

9.37 

50 

16.77 

69 

27.84 

Lead  permanganate. 
Sol.  in  HNO3+Aq.    (Forchhammer.) 

13 
14 
15 

4.98 
5.18 
5.38 

32 
33 
34 

9.69 
10.01 
10.34 

51 
52 
53 

17.23 
17.71 
18.21 

70 
71 

72 

28.56 
29.30 
30.05 

16 

5.60 

35 

10.68 

54 

18.71 

73 

30.81 

Lithium  permanganate,  LiMnO4+3H2O. 
Sol.  in  1.4  pts.  H2O  at  16°.    (Aschoff.) 

17 

18 

5.82 
6.04 

36 
37 

11.02 
11.38 

55 
56 

19.23 
19.75 

74 
74.5 

31.57 
31.95 

Magnesium  permanganate,  Mg(MnO4)2. 

Insol.  in  CHC13,  CC14,  C6H6,  toluene,  nitro- 
benzene, ligroin,  ether  and  CS2.  Sol.  in 
methyl  alcohol,  acetone,  pyridine,  and  readily 
sol.  in  glacial  acetic  acid.  Only  pyridine  and 
glacial  acetic  acid  are  sufficiently  stable  to- 
ward the  salt  to  be  of  any  practical  use  for 
oxidation  purposes.  (Michael  and  Garner, 
Am.  Ch.  J.  1906,  35.  268.) 

+6H2O.    Easily  deliquescent. 

Nickel  permanganate  ammonia.  Ni(MnO4)2, 

4NH3. 

Sol.  in  H2O  with  decomp.  (Klobb,  Bull. 
Soc.  (3)  3.  509.) 

Potassium  permanganate,  KMnO4. 


(Worden,  J.  Soc.  Chem.  Ind.  1907,  26.  453.) 

Solubility  in  H2O. 

100  com.  of  the  sat.  solution  contain  at: 
0°         15°       15.3°        30° 
2.84      5.22         5.30      8.69  g.  KMnO4. 
Sp.    gr.    of    sat.    solution    at    15°  =  1.035. 
(Patterson,    J.   Am.    Chem.    Soc.    1906,    28. 
1735.) 

1  1.  sat.  KMnO4+Aq  contains  at: 
0°       10°      20°      30°      40° 
0.176  0.278  0.411   0.573  0.792  mol.  KMnO4, 

53°         63°         70°         75° 
1.154      1.429      1.812      2.047  mol.  KMnO4. 
(Sackur,  Z.  Elektrochem.  1912,  18.  723.) 

Solubility  of  KMnO4  in  H2O  at  t°. 


DQI.  in  ID  pts.  ±12U  at  15  .    (Mitscnerlicn.j 
Solubility  in  100  pts.  H2O  at  t°. 

Grams  KMnCU  sol.  in 
100  grams  H2O 

t° 

0.58 
1.01 

2.02 
2.91 
4.22 
5.20 
7.53 
11.61 
16.75 

-0.18 

t° 

Pts.  KMnO4 

—  0.27 
—  0.48 
—  0.58 
+10 

+  15 
+25 
+40 
+50 

0 
9.8 
19.8 
24.8 
29.8 
34.8 
40.0 
45.0 
50.0 
55.0 
65.0 

2.83 
4.31 
.  6.34 
7.59 
9.03 
10.67 
12.56 
14.58 
16.89 
19.33 
25.03 

(Voerman,  C.  C,  1906,  I.  125.) 

Sol.  in  cone.  H2SO4.    Deliquesces  in  liquid 
HC1,  but  does  not  dissolve.    (Gore.) 
Slowly  sol.  in  H3PO4+Aq.     (Chevillot  and 
Edwards.) 

(Baxter,  J.  Am.  Chem.  Soc.  1906,  28.  1343.) 

PERMANGANATE  AMMONIA,  SILVER 


659 


Solubility  in  KOH+Aq  at  t°  expressed  in  mol.  per  1.  of  the  sat.  solution. 


t° 

H20 

l-n  KOH 

2-n  KOH 

4-n  KOH 

6-n  KOH 

8-n  KOH 

10-n  KOH 

0 

0.176 

0.050 

0.031 

0.027 

0.023 

0.017 

0.012 

10 

0.278 

0.112 

0.068 

0.048 

0.042 

0.028 

0.016 

20 

0.411 

0.179 

0.119 

0.079 

19°  0.074 

0.032 

0.029 

30 

0.573 

32°  0.316 

32°  0.213 

32°  0.149 

0.114 

32°  0.062 

0.040 

40 

0.792 

0.439 

0.306 

0.211 

0.161 

0.084 

0.052 

50 

53°  1.154 

50°  0.638 

0.462 

0.304 

0.219 

0.111 

63 

1.429 

61°  0.904 

60°  0.639 

0.427 

0.291 

61°  G.143 

0'071 

70 

1.812 

1.172 

0.869 

0.572 

0.390 

0.188 

0.082 

75 

2.047 

0.651 

0.089 

80 

1.513 

ivioo 

0^500 

0*231 

84 

1.655 

1.352 

83°  0^803 

85°  0.572 

90 



0.649 

0^297 

(Sackur,  Z.  Elektrochem.  1912,  18.  723.) 


Solubility  in  salts  +Aq.  at  t°. 

Solubility  in  ace 

bone+Aq.  at  13°. 
100  ccm.  acetone  +Aq. 
s  KMnO4  in  100  ccm. 

Solvent 

t° 

Mol.  KMnO4 
in  1  1.  of  sat. 
solution 

A—  ccm.  acetone  in 
1/6KMnO4=millimol 
of  the  solution. 

0  ^K.CO, 

0 
25 

40 

0.1462 
0.4375 
0.7380 

A 

1/5  KMnO4 

2 

0 
10 
20 
30 
40 
50 
60 
70 
80 
90 
100 

148.5 
162.2 
177.3 
208.2 
257.4 
289.7 
316.8 
328.0 
312.5 
227.0 
67.6 

l-n  5-92.' 

0 
25 

40 

0.0629 
0.2589 
0.5007 

2-n  5*22.' 

2 

0 
40 

0.0446 
0.3519 

^K.00.       ' 

0 
25 

0.0270 
0.0930 

(Herz  and  Knoch,  Z.  anorg.  1904,  41.  317.) 

Sol.  in  benzonitrile.     (Naumann,  B.  1914, 
47.  1369.) 
Difficultly  sol.  in  methyl  acetate,     (Nau- 
mann, B.  1909,  42.  3795.) 
Sol.  in  ethyl  acetate.    (Naumann,  B.  1904, 
37.  3601.) 

Rubidium  permanganate,  RbMnO4. 
Solubility  in  H2O  lies  between  K  and  Cs 
salts.    (Muthmann,  B.  1893,  26.  1018.) 
Solubility  in  H2O. 
100  ccm.  of  the  sat.  solution  contain  at: 
2°           19°          60° 
0.46         1.06        4.68  g.  RbMnO4. 
(Patterson,    J.   Am.   Chem.   Soc.    1906,   28. 
1735.) 

fl^K.CO. 
2 

0 

0.0156 

0.1-nKCl 

0 
25 

40 

0.1395 
0.4315 
0.7380 

0.5-nKCl 

0 
25 

40 

0.0760 
0.3060 
0.5840 

1-nKCl 

0 
25 
40 

0.0532 
0.220 
0.444 

2-nKCl 

0 
25 

40 

0.0379 
0.1432 

0.288 

(Sackur,  Z.  Elektrochem.  1912,  18.  723.) 

Very  sol.  in  liquid  NH3.  (Moissan,  A.  ch. 
1895  (7)  6.  428;  Franklin,  Am.  Ch.  J.  1898, 
20.  829.) 

Decomp.  immediately  by  alcohol.  Sol.  in 
acetone.  (Eidmann,  C-.  C.  1899.  II,  1014; 
Naumann,  B.  1904,  37.  4328.) 


Sol.  in  109  pts.  cold  H2O  and  much  less  hot 
H->O.  Decomp.  by  boiling.  (Mitscherlich, 
>ogg.  25.  301.) 

Silver  permanganate  ammonia. 

SI.  sol.  in  cold,  more  easily  in  hot  H2O. 
Klobb,  C.  R.  103.  384.) 


660 


PERMANGANATE,  SODIUM 


Sodium  permanganate,  NaMnO4+3H2O. 

Deliquescent.    Extremely  sol.  in  H2O. 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  829.) 

Strontium  permanganate,  Sr(MnO4)2+4H2O. 
Deliquescent.    Sol.  in  H2O.    (Fromherz.) 

Thallous  permanganate,  TlMnO4. 

Sol.  in  H2O  with  decomp.  (R.  Meyer,  Z. 
anorg.  1899,  22.  188.) 

Zinc  permanganate,  Zn(MnO4)2+6H2O. 

Deliquescent.  Very  sol.  in  H2O.  (Marten- 
son,  J.  B.  1873.  274.)^ 

Zinz  permanganate  ammonia, 

Zn(MnO4)2,  4NH3. 

Sol.  in  H2O  with  decomp.  (Klobb,  Bull. 
Soc.  (3)  3.  509.)' 

Permanganomolybdic  acid,  MnO2, 

12MoO3+10H2O. 

Sol.  in  H2O.  Decomp.  by  alkalis.  Sol.  in 
alcohol.  (Pochard,  C.  R.  1897,  125.  31.) 

Ammonium  permanganomolybdate, 
2(NH4)2O,  MnO2,  7MoO3+5H2O. 

(Friedheim  and  Samelson,  Z.  anorg.  1900, 
24.  73.) 

3(NH4)2O,  MnO2,  9MoO3+6H2O.  (Fried- 
heim and  Allemann,  Mit.  d.  Nat.  Ges.  Bern. 
1904.  23.) 

+7H2O.  (Friedheim  and  Samelson,  Z. 
anorg.  1900,  24.  70.) 

4(NH4)2O,  MnO2,  HMoO3+7H2O.  (Fried- 
heim and  Samelson.) 

3(NH4)2O,  MnO2,  12Mo03+5H2O.  SI. 
sol.  in  cold  H2O.  Decomp.  by  alkalis.  Insol. 
in  alcohol.  (Pochard,  C.  R.  1897,  125.  30.) 

Ammonium  manganous  permanganomolyb- 
date, 3[(NH4)2,  Mn]O,  MnO2,  9MoO3  + 
6H2O  and  +7H2O. 

(Friedheim  and  Allemann,  Mitt.  d.  Nat. 
Ges.  Bern.  1904.  23.) 

3](NH4)2,  Mn]O,  MnO2,  10MoO3+10H2O. 
(Friedheim  and  Samelson,  Z.  anorg.  1900,  24. 
94.) 

4[(NH4)2,  Mn]O,  MnO2,  10MoO3+6H2O. 
(Friedheim  and  Samelson,  Z.  anorg.  1900,  24. 
75.) 

4[(NH4)2,  Mn]O,  MnO2,  HMoO3+8H2O. 
(Friedheim  and  Samelson,  Z.  anorg.  1900,  24. 
72.) 

Ammonium  manganous  potassium  perman- 
ganomolybdate, 2(NH4)2O,  MnO,  K20, 
MnO2,  10MoO3+5H2O. 
Very  si.  sol.  in  cold,  easily  sol.  in  H2O  at 
70-80°.    (Rosenheim,  Z.  anorg.  1898,  16.  79.) 
3[(NH4)2,    K2,    Mn]O,    MnO2,    9MpO3-f 
7H2O.     (Friedheim  and  Allemann,  Mitt.  d. 
Nat.  Ges.  Bern.  1904.  23.) 


4[(NH4)2,  K2,  Mn]O,  MnO2,  10MoO3-f 
5H2O.  (Friedheim  and  Samelson,  Z.  anorg. 
1900,  24.  97.) 

3[(NH4)2,  K2,  Mn]O,  MnO2,  10MoO3-f 
6H2O,  and  +  10H2O.  (Friedheim  and  Samel- 
son, Z.  anorg.  1900,  24.  92.) 

Ammonium  potassium  permanganomolyb- 
date, 3[(NH4)2,  K2]O,  MnO2,  8MoO3  + 
4H2O. 

(Friedheim  and  Samelson.) 

Barium  permanganomolybdate,  3BaO,  MnO2, 

9MoO3  +  12H2O. 

Ppt.  (Hall,  J.  Am.  Chem.  Soc.  1907,  29. 
700.) 

Manganous  potassium  permanganomolyb- 
date, 2K2O,  MnO,  MnO2,  9MoO3  + 
8H20. 

True  formula  for  5K2O,  Mn2O3,  16MoO3+ 
12H2O  of  Struve.  (Friedheim  and  Samelson, 
Z.  anorg.  1900,  24.  86.) 

3[K2,Mn]O,  MnO2,  9MoO3+6H2O.  (Fried- 
heim and  Allemann,  Mitt.  d.  Nat.  Ges.  Bern. 
1904.  23.) 

2.6  K2O,  0.4  MnO,  MnO2,  9MoO3+7H2O. 
Ppt.  (Hall,  J.  Am.  Chem.  Soc.  1907,  29. 
700.) 

4[K2,  Mn]O,  MnO2,  HMoO3+7H20. 
(Friedheim  and  Samelson,  Z.  anorg.  1900,  24. 
80.) 

Manganous  potassium  sodium  permangano- 
molybdate,  3[K2,   Na2,     MnjO,    MnO2, 
8MnO3+4H2O. 
(Friedheim  and  Allemann,  Mitt.  d.  Nat. 

Ges.  Bern.  1904.  48.) 

Manganous   sodium  permanganomolybdate, 

3[Na2,  MnjO,  MnO2,  9MoO3  +  15H2O. 
(Friedheim  and  Allemann.) 

Potassium   permanganomolybdate,   3K2O, 
MnO2,  8MoO3+3H2O. 

Much  less  sol.  in  H2O  than  NH4  comp. 
(Friedheim  and  Samelson,  Z.  anorg.  1900,  24. 
78.) 

-|-5H2O.  Nearly  insol.  in  cold  or  hot  H20. 
(Rosenheim  and  Itzig,  Z.  anorg.  1898,  16.  81.) 

3K2O,  MnO2,  9MoO3+5H2O.  (Friedheim 
and  Samelson,  Z.  anorg.  1900,  24.  81.) 

+6H2O.  (Hall,  J.  Am.  Chem.  Soc.  1907, 
29.  700.) 

3K2O,  MnO2,  12MoO3+4H2O.  Nearly 
insol.  in  cold  H2O.  Decomp.  by  alkalis. 
Insol.  in  alcohol.  (Pochard,  C.  R.  1897,  125. 
31.) 

Silver  permanganomolybdate,  3Ag2O,  MnO2, 

9MoO3+6H2O. 

Ppt.  (Hall,  J.  Am.  Chem.  Soc.  1907,  29. 
700.) 


PEROXYNITRATE,  SILVER 


661 


Sodium  permanganomolybdate,  3Na2O, 

MnO2,  12MoO3  +  13H2O. 
Efflorescent.    Very  sol.  in  H2O.     Decomp. 
hv  alkalies.   Insol.  in  alcohol.    (Pechard,  C.  R. 
125.  31.) 

Permanganotungstic  acid. 

Ammonium  manganous  permanganotung- 
state,  4(NH4)2O,  MnO,  MnO2,  12WO3+ 
23H2O. 

Readily  sol.  in  H2O.  Can  be  cryst.  there- 
from. (Rogers  and  Smith,  J.  Am.  Chem. 
Soc.  1904,  26.  1475.) 

Sodium  permanganotungstate,  3Na2O,  MnO2, 

5WO3  +  18H2O. 

Rather  easily  sol.  in  hot  H2O.  Solution 
decomp.  on  long  boiling  with  separation  of 
manganese  peroxide.  (Just,  B.  1903,  36. 
3621.) 

Permolybdic  acid,  Mo2O7,  5H2O  = 
HMoO4+2H2O. 

Verv  sol.  in  H2O,  and  not  decomp.  by  boil- 
.  ing.  (Pechard,  A.  ch.  (6)  28.  550.) 

H2MoO5  +  lKH2O.  "Ozo-molybdic  acid." 
Only  very  si.  sol.  in  H2O  after  being  dried  in 
the  air.  801.  in  fairly  cone.  H2SO4.  (Muth- 
mann, B.  1898,  31.  1838.) 

H2Mo2O7,  H2O2.  SI.  sol.  in  cold,  more  eas- 
ily sol.  in  hot  H2O,  but  does  not  separate  on 
cooling.  Sol.  in  dil.  acids,  also  in  H3PO4. 
(Cammerer,  Ch.  Z.  1891,  15.  957.) 

Ammonium    permolybdate,     NH4MoO4+ 
2H2O. 

Very  sol.  in  H2O;  si.  sol.  in  alcohol,  but 
alcohol  extracts  it  from  H2O,  forming  a  very 
cone,  supersat.  solution,  which  is  pptd.  by  a 
crystal  of  NH4MoO4,  and  only  a  si.  amount 
remains  in  solution.  (Pochard.) 

3(NH4)2O,  5MoO3,  2MoO4+6H2O.  (Muth- 
mann,  B.  1898,  31.  1837.) 

3(NH4)2O,  7MoO4+12H2O.  Ppt.  (Muth- 
mann,  Z.  anorg.  1898,  17.  76.) 

3(NH4)20, 5MoO4+6H2O.  Ppt.  (Muth- 
mann.) 

Ammonium    nickel  permolybdate  ammonia 

(NH4)2Ni(MoO4)2,2NH3. 
Decomp.  by  H2O.     Sol.  in  dil.  NH4OH. 
(Briggs,  Chem.  Soc.  1904,  85.  674.) 

Barium  permolybdate,  Ba(MoO4)2+2H2O. 
(Pechard,  A.  ch.  1893,  (6)  28.  537.) 
8BaO,    19MoO3,    2H2O2  +  13H2O.      (Baer- 

wald,  Dissert.  1885.) 

Caesium  permolybdate,  Cs2O,  4MoO4+6H2O. 

Sol.  hot  HoO.  (Muthmann,  B.  1898,  31. 
1841.) 

3Cs2O,  7MoO3,  3MoO4+4H2O.     Ppt. 
(Muthmann.) 


Copper  permolybdate,  Cu(MoO4)2+H2O. 

Insol.  in  H2O;  easily  sol.  in  acids.  Sol.  in 
NH4OH+Aq  with  decomp.  (Pechard.) 

Magnesium     permolybdate,     Mg(MoO4)2  + 

10H2O. 

Very  sol.  in  H2O;  si.  sol.  in  alcohol.  (Pech- 
ard.) 

Mercurous  permolybdate. 

Insol.  in  H2O  or  NH4NO3  + Aq.    (Pechard.) 

Potassium  permolybdate,  KMoO4+2H2O. 

SI.  sol.  in  cold,  more  in  hot  H2O.  SI.  sol! 
in  alcohol.  (Pechard.) 

K2O,2MoO3,  MoO4+3H2O.  Ppt,  (Muth- 
mann, Z.  anorg.  1898,  17.  77.) 

K2O2,  MoO4,  H2O2.  Decomp.  by  H2O. 
(MelikofT  and  Pissarjewsky,  B.  1898,  31. 
2449.) 

K2MoO5+3H2O.  Nearly  insol.  in  cold, 
easily  sol.  in  hot  H2O.  (Mazzuchelli  and 
Zangrilli,  Gazz.  ch.  it.  1910,  40.  (2)  56.) 

Rubidium  permolybdates. 

' '  Rubid  ium  ozo-molybdate. ' ' 

3Rb2O,  10MoO4+14H2O.    Ppt. 

Rb2O,  2MoO3,  MoO4+3H2O.  May  be  re- 
cryst.  from  H2O2-f-Aq. 

3Rb2O,  5MoO3,  2MoO4+6H2O.    Ppt. 

Rb2O,  3MoO3,  MoO4+4H2O.  Ppt.  (Muth- 
mann, B.  1898,  31.  1839-41.) 

Silver  permolybdate,  AgMoO4. 

.  (Pechard.) 

Sodium  permolybdate,  NaMoO4+3H2O. 

Very  sol.  in  H2O;  insol.  in  alcohol,  but 
behaves  similarly  to  K  salt.  (Pechard.) 

Thallous  permolybdate. 

Insol.  in  H2O.  (Pochard,  A.  ch.  1893,  (6) 
28.  559.) 

Pemitric  acid,  NO3. 

See  Nitrogen  hexoxide. 

Silver  pernitrate,  basic,  3Ag2O2,  AgNO5. 

Decomp.  H2O.  (Mulder,  R.  t.  c.  1898,  17. 
142.) 

Perosmic  acid. 

Potassium  perosmate  (?). 

Sol.  in  H2O,  but  very  easily  decomp. 

Peroxynitric  acid. 

Silver  peroxynitrate. 

Analysis  of  the  black  compound  formed, 
under  certain  circumstances,  in  a  silver  volt- 
ameter when  an  aqueous  solution  of  AgNO3 


662 


PEROXYLAMINE  SULPHONIC  ACID 


is  electrolyzed,  points  to  the  composition 
3Ag2O,  5O,  AgNO3,  perhaps  2Ag,O4,  AgNO8 
or  3Ag2O2,  AgNO5.  (Mulder,  Chem.  Soc. 
1896,  70.  (2)  561.) 

Peroxylaminesulphonic  acid. 


Potassium  peroxylaminesulphonate, 

N2O2(SO3K)4. 

Very  unstable  in  H2O.  Very  si.  sol.  in  cold 
H2O.  'More  stable  in.N/10  KOH+Aq. 

100  pts.  N/10  KOH+Aq  dissolve  0.62  pt. 
of  the  salt  at  3°;  6.6  pts.  at  29°.  (Haga, 
Chem.  Soc.  1904,  86.  86.) 

Perstannic  acid,  H2Sn2O7. 

Known  in  colloidal  state,  sol.  in  H2O. 
(Spring,  Bull.  Soc.  (2)  51.  180.) 

Potassium  perstannate,  KSnO4+2H2O. 

Sol.  in  H2O.  Insol.  in  alcohol.  (Tanatar, 
B.  1905,  38.  1185.) 

Sodium  perstannate,  NaSnO4+2H20. 

Difficultly  sol.  in  H2O  with  decomp. 
(Tanatar.) 


Persulphuric 

See  Sulphur  heptoxide. 

H2S208. 


Sp.  gr.  of  H2S208+Aq. 


Ammonium  lead  persulphate, 

(NH4)2Pb(S04)3. 
Decomp.  by  H2O.  Almost  insol.  in  cold 
H2S04  of  sp.  gr.  =  1.7.  SI.  sol.  in  H2SO4  (sp. 
gr.  =  1.7)  at  50°.  Sol.  in  fuming  H?SO4  and 
in  cold  cone.  HC1.  Sol.  in  acetic  acid,  in  Na 
acetate +Aq  acidified  with  acetic  acid  and  in 
excess  of  cold  20%NaOH+Aq.  (Elbs,  Z. 
Elektrochem.  1900,  7.  346.) 


Ammonium     mercurous     persulphate     am- 
monia, (NH4)HgS2O8,  2NH3. 
Decomp.  by  H2O.     Insol.  in  dil.  or  cone., 
hot  or  cold  H2SO4  or  HNO3.     Sol.  in  HC1. 
(Tarugi,  Gazz.  ch.  it.  1903,  33.  (1)  131.) 

Barium  persulphate,  BaS2O8+4H2O. 

Very  sol.  in  H2O.  100  pts.  H2O  at  0°  dis- 
solve 39.1  pts.  BaS2O8,  or  52.2  pts.  BaS2O8+ 
4H2O.  Sol.  in  absolute  alcohol  with  pptn.  of 
BaS2O8+H2O.  Insol.  in  alcohol.  (Marshall.) 

Cadmium    persulphate    ammonia,    CdS2O8, 

6NH3. 

Sol.  in  H2O.  (Barbieri,  Z.  anorg.  1911.  71. 
350.) 

Caesium  persulphate,  Cs2S2O8. 

Sol.  in  H2O.  8.71-8.98  pts.  are  sol.  in  100 
pts.  H2O  at  23°.  (E.  F.  Smith,  J.  Am.  Chem. 
Soc.  1899,  21.  935.) 

Calcium  persulphate. 

Very  sol.  in  H2O.  (Marshall,  J.  Soc.  Chem. 
Ind.  1897,  16.  396.) 

Copper  persulphate  ammonia,  CuS2O8,  4NH8. 
Sol.  in  H2O.    (Barbieri,  Z.  anorg.  1911,  71. 
351.) 

Lead  persulphate,  PbS2O8. 

Decomp.  by  H2O.  SI.  sol.  in  H2SO4,  and  in 
pyrosulphuric  acid.  Sol.  in  cold  cone.  HC1. 
Insol.  or  sol.  with  decomp.  in  all  ord.  solvents. 
(Elbs,  Z.  Elektrochem.  1900,  7.  345.) 


Sp.  gr.  14°/14° 

%  H2S208 

g.  HzSzOs  per  1. 

Solubility  of  Pb(SO4)2  in  H2SO4+Aq.  at  22°. 

1.042 

7.2 

75 

v=  moles    of    H2SO4    per    mole    of    H2O; 

1.096 

15.4 

169 

c=millimols  Pb(SO4)2  in  1  1. 

11  K.A 

OQ    £\ 

979 

.  1O'± 

1.246 

35'2 

&%  & 

438 

V 

C 

V 

C 

(Elbs  and.  Schonherr,  Z.  Elektrochem.  1896, 

0.304 

0.00 

0.558 

37.2 

2.  245.) 

0.348 

1.8 

0.699 

40.5 

0.387 

3.0 

0.917 

23.3 

Ammonium  persulphate,  (NH4)2S2O8. 
Very  sol.  in  H2O.     100  pts.  H2O  at  0°  dis- 
solve   58.2    pts.     (NH4)2S2O8.       (Marshall, 
Chem.  Soc.  59.  771.) 

0.407 
0.435 
0.477 
0.515 

3.9 
5.3 
14.4 
23.3 

1.11 
1.54 
2.08 
2.13 

23.7 
49.6 
83.5 

88.2 

Solubilitv    in    H2O    equals    58%    at    8°. 
(Moreau,  C.  C.  1901,  II.  56.) 

(Dolezalek  and  Finckli,  Z.  anorg.  1906,  51. 
321.) 

100  pts.  H2O  dissolve  65  pts.  at  ord.  temp. 

(Elbs,  J.  pr.  1893,  (2)  48.  185.) 

+3H2O.    Deliquescent.    Very  sol.  in  H20. 

(Marshall.) 

Lead  potassium  persulphate,  K2Pb(SO4)3. 

Decomp.  by  H2O.  Almost  insol.  in  cold 
H2SO4  of  sp.  gr.  =  1.7.  SI.  sol.  in  H2S04  (sp 
gr.  =  1.7)  at  50°.  Sol.  in  fuming  H2SO4,  cole 
cone.  HC1,  excess  of  cold  20%  NaOH+Aq 
acetic  acid,  and  in  Na  acetate +Aq  acidifiec 
with  acetic  acid.  (Elbs,  Z.  Elektrochem 
1900,  7.  346.) 


PERTUNGSTATE,  LITHIUM 


663 


Nickel  persulphate  ammonia,  NiS2O8,  6NH 

Unstable  in  the  air.    Sol.  in  H2O  with  de- 
comp.    (Barbieri,  Z.  anorg.  1911,  71.  351.) 


Potassium  persulphate, 

100  pts.  H2O  at  0°  dissolve  1.77  pts.  K2S2O; 
more  sol.  in  hot  H2O  with  very  si.  decomp 
Less  sol.  in  H2O  than  any  other  persulphate 

(Marshall.) 

Rubidium  persulphate,  Rb2S2O8. 

Sol.  in  H2O.  3.32-3.49  pts.  are  sol.  in  10( 
pts.  H2O  at  22.5°.  (E.  F.  Smith,  J.  Am 
Chem.  Soc.  1899,  21.  934.) 

Silver  persulphate,  basic,  5Ag2O2,  2Ag2SO7. 

Decomp.  by  H2O  and  acids.  (Mulder,  C.  C 
1899.  I,  16.) 

Sodium  persulphate,  Na2S2O8. 
Very  sol.  in  H2O.    (Lowenherz.) 

Strontium  persulphate. 

Very  sol.  in  H2O.  (Marshall,  J.  Soc.  Chem 
Ind.  1897,  16.  396.) 

Thallium  persulphate,  T12S2O8. 

Very  sol.  in  H2O.  (Smith,  J.  Am.  Chem 
Soc.  1898,  21.  936.) 

Zinc  persulphate  ammonia,  ZnS2O8,  4NH3. 

Sol.  in  H2O.  (Barbieri,  Z.  anorg.  1911,  71 
350.)  . 

Persulphomolybdic  acid. 
See  Persulphomolybdic  acid. 

Pertantalic  acid,  HTaO4-f-nH2O. 

Ppt.    (Melikoff,  Z.  anorg.  1899,  20.  345.) 

Caesium  pertantalate,  Cs3TaO8. 

Ppt.  (E.  F.  Smith,  J.  Am.  Chem.  Soc. 
1908,  30.  1667.) 

Calcium  potassium  pertantalate.  CaKTaO8+ 

43^H20. 

Insol.  in  cold  H2O;  decomp.  by  hot  H2O. 
(Melikoff,  Z.  anorg.  1899,  20.  3470 

Calcium  sodium  pertantalate,  CaNaTaO8+ 


Difficultly  sol.  in  H2O.     (E.  F.  Smith,  J. 
Am.  Chem.  Soc.  1908,  30.  1668.) 

Magnesium  potassium  pertantalate, 

MgKTaO8+7H2O. 
Somewhat  sol.  in  H2O.    (E.  F.  Smith.) 

Magnesium  rubidium  pertantalate, 

MgRbTa08+9H2O. 
Somewhat  sol.  in  H2O.    (E.  F.  Smith.) 


Magnesium  sodium  pertantalate,  MgNaTaOs 

+8H20. 
Somewhat  sol.  in  H2O.    (E.  F.  Smith.) 

Potassium  pertantalate, 

Sol.  in  H2O  with  decomp.;  sol.  in  KOH+ 
H2O2+Aq;  pptd.  by  alcohol.  (Melikoff,  Z. 
anorg.  1899,  20.  346.) 

Rubidium  pertantalate,  Rb3TaO8. 

Somewhat  sol.  in  H2O.    (E.  F.  Smith.) 

Sodium  pertantalate,  Na3TaO8+H2O. 

Pptd.  by  alcohol.  SI.  sol.  in  H2O,  decomp. 
on  heating  with  H2O.  (Melikoff,  Z.  anorg. 
1899,  20.  348.) 

NaTaO4+NaOTaO4+13H2O.  Sol.  in 
H2O2+Aq;  pptd.  by  alcohol.  (Melikoff,  Z. 
anorg.  1899,  20.  349.) 

Pertitanic  acid. 

Ammonium   pertitanate,    (NH4)2O2,    TiO3-f 

H202. 

Fairly  stable;  decomp.  rapidly  in  aq.  solu- 
tion. (Melikoff,  B.  1898,  31.  955.) 

Barium  pertitanate,  BaO2,  TiO3+5H2O. 

SI.  sol.  in  H2O.  (Melikoff  and  Pissarjew- 
sky,  Z.  anorg.  1898,  18.  59.) 

Potassium  pertitanate,  K2O2,  TiO3,  K2O4+ 

10H2O. 

Stable  at  zero;  deliquesces  and  decomp.  at 
ordinary  temp.  (Melikoff,  B.  1898,  31.  680.) 

Sodium  pertitanate,  Na2O2,  TiO3+3H2O. 

Sol.  in  H2O.  Pptd.  in  alcohol.  (Melikoff, 
B.  1898,  31.  955.) 

4Na2O2,  Ti2O7+10H2O.  Decomp.  by  H20. 
[Melikoff.) 

Pertungstic  acid. 

Barium  pertungstate,  BaO,  2WO3,  O+6H2O. 
Insol.  in  H2O.  Decomp.  by  acids.  (Kell- 
ner,  Dissert.  1909.) 

Caesium  pertungstate,  3Cs2O,  12WO3,  2O  + 

12H2O. 

SI.  sol.  in  cold,  easily  sol.  in  warm  H2O. 
Kellner.) 

5Cs2O,  12WO3,  24O  +  11H2O. 
SI.  sol.  in  H2O.    (Kellner.) 

Calcium   pertungstate,   3CaO,    6WO3,   8O  + 

8H2O. 
Sol.  inH2O.    (Kellner.) 

,ithium  pertungstate,  Li2O,  2WO3,  2O-f- 
6H20. 

SI.  sol.  in  H2O.    (Kellner.) 

3Li2O,  4WO3,  O+9H2O.  Sol.  in  H20. 
KeUner.) 


664 


PERTUNGSTATE,  MAGNESIUM 


Magnesium  pertungstate,  2MgO,  4WO3,  6O  + 

9H2O. 
Easily  sol.  in  H2O.    (Kellner.) 

Potassium  pertungstate,  K2O4,  WO4+H2O. 

Sol.  in  H2O  with  decomp.;  explodes  in  the 
air  at  80°.  (Melikoff,  B.  1898,  31.  634.) 

K2O,  2WO3,  4O+4H20.  Sol.  in  H2O  from 
which  it  is  ppt.  by  alcohol  and  ether.  (Kell- 
ner.) 

7K2O,  10WO3,  5O+22H2O.  Very  si.  sol. 
inH20.  (Kellner.) 

Rubidium  pertungstate,  2Rb2O,  4WO3,  O  + 
3H2O. 

Sol.  in  H2O  with  slow  decomp.    (Kellner.) 

5Rb2O,    12W( 
H2O.    (Kellner.) 


5Rb2O,    12WO3,    3O  +  12H2O.      Insol.    in 


nap. 
.0. 


Sodium  pertungstate,  NaWO4+H2O. 

Very  sol.  in  H2O.  (Pechard,  C.  R.  112. 
1060.) 

+2H2O.  Sol.  in  H2O  but  easily  decomp. 
(Kellner.) 

Na2W2O9-f-6H2O.  Sol.  in  H2O  and  can 
be  cryst.  therefrom.  (Pissarjewsky,  Z.  anorg. 
1900,  24.  113.) 

Na202,  W04+H202,  (Na202)W04+7H20. 
Decomp.  in  the  air.    Sol.  in  H2O  with  decomp. 
(Melikoff,  B.  1898,  31.  633.) 

Na2Q2,  WO4,  H2O2.  Very  unstable.  De- 
comp. in  the  air  and  by  H2O.  (Melikoff.) 

Strontium    pertungstate,    SrO,    2WO3,    O  + 

6H20. 
(Kellner.) 

Peruranic  acid,  UO6,  zH2O  (?). 
Known  only  in  its  salts. 

Ammonium  peruranate,  (NH4)2O2,  (UO4)2  + 

8H2O. 

Sol.  in  H20;  decomp.  by  acids  and  by 
A1(OH)3  in  aq.  solution.  (Melikoff,  B.  1897, 
30.  2904.) 

Ammonium  uranyl  peruranate, 

(NH4)2(UO2)UO8+8H2O  (?). 
Easily  sol.  in  H2O.     (Fairley,  Chein.  Soc. 
(2)  31.  134.) 

Barium  peruranate,  BaUO5. 

As  K  salt,  (de  Coninck,  C.  C.  1909,  I. 
1970.) 

(Ba02)2UO4+8H20.  Decomp.  by  H2S04 
and  H2C08.  (Melikoff,  B.  1897,  30.  2905.) 

BaO2(UO4)2+9H2O.    Ppt.    (Melikoff.) 

Calcium  peruranate,  CaUO5. 

As  K  salt,    (de  Coninck.) 

Calcium  peruranate,  (CaO2)2UO4+10H2O. 
Ppt.    (Melikoff,  B.  1897,  30.  2906.) 


Copper  peruranate,  (CuO2)2UO4. 
Ppt.  (Melikoff.) 

Lead  peruranate,  (PbO)2UO4,  PbO,  UO3. 
Ppt.    (Melikoff.) 

Lithium  peruranate,  (Li2O2)(UO4)2+8H2O. 

Sol.  in  H2O;  decomp.  by  acids  and  by 
A1(OH)3  in  aq.  solution;  very  unstable. 
(Melikoff.) 

Nickel  peruranate,  (NiO)2UO4. 
Ppt.    (Melikoff.) 

Potassium  peruranate,.  K4UO8  +  10H2O  (?). 

Unstable.    (Fairley.) 

K2UO6.  (de  Coninck,  C.  R.  1909,  148. 
1769.) 

+3H2O.  Decomp.  by  H2O,  HC1  and  dil. 
HNO3.  (Aloy,  Bull.  Soc.  1903,  (3)  29.  293.) 

Silver  peruranate,  Ag2U2On  (?). 
(Guyard,  Bull.  Soc.  (2)  1.  95.) 
Does  not  exist.  (Alibegoff,  A.  233.  117.) 

Sodium  peruranate,  Na4UO8+SH2O. 

Sol.  in  H2O.    SI.  sol.  in  alcohol.    (Fairley.) 

Na2UO5.  As  K  salt,  (de  Coninck,  C.  C. 
1909,  I.  1970.) 

+5H2O.  Decomp.  by  H2O  and  HC1. 
(Aloy,  Bull.  Soc.  1903.  (3)  29.  293.) 

(Na2O2)2UO4-f-8H20.  Sol.  in  H2O;  de- 
comp. by  dil.  HC1,  H2S04,  and  by  Al(OH)t 
in  aq.  solution.  (Melikoff,  B.  1897,  30.  2903.) 

Sodium  uranyl  peruranate,  Na2(UO2)UO8+ 

6H2O  (?). 
Sol.  inH2O.    (Fairley.) 

Pervanadic  acid,  HVO4  (?). 

Sol.  in  H2O.  (Pissarjewsky,  C.  C.  1902,  II. 
565.) 

Ammonium  pervanadate,  NH4VO4. 

Sol.  in  H2O2+Aq;  insol.  in  alcohol.  (Scheuer 
Z.  anorg.  1898,  16.  294.) 

(NH4)3VO6+2^H2O.  Sol.  in  H2O;  insol. 
in  alcohol.  (Melikoff,  B.  1909,  42.  2292.) 

(NH4)4V2On.  Sol.  in  H2O2-f-Aq;  ppt.  from 
aq.  solution  by  alcohol.  (Melikoff,  Z.  anorg. 
1899,  19.  406.) 

Barium  pervanadate,  Ba(VO4)2. 

SI.  sol.  in  H202+Aq  free  from  H2SO4; 
insol.  in  alcohol.  (Scheuer,  Z.  anorg.  1898, 
16.  288.) 

Cadmium  pervanadate,  Cd(VO4)2. 

SI.  sol.  in  H2O2+Aq;  insol.  in  alcohol. 
(Scheuer.) 

Calcium  pervanadate,  Ca(VO4)2. 

Sol.  in  H2O2+Aq;  insol.  in  alcohol. 
(Scheuer.) 


PHOSPHIMATE,  BARIUM 


665 


Lead  pervanadate,  Pb(VO4)2. 

SI.  sol.  in  H2O2+Aq  free  from  H2SO4;  insol. 
in  alcohol.  (Scheuer.) 

Lithium  pervanadate,  LiVO4. 

Sol.  in  H2O2  +Aq;  insol.  in  alcohol. 

(Scheuer.) 

Potassium  pervanadate,  KVO4. 

Sol.  in  H2O2+Aq  acidified  with  H2SO4; 
insol.  in  alcohol.  (Scheuer.) 

K8VO8+2^H2O.  Sol.  in  H2O;  insol.  in 
alcohol.  (Melikoff,  B.  1909,  42.  2293.) 

3K202V04,  2KV04+2H2O.  0.855  g.  is 
sol.  in  100  g.  H2O  at  19°;  si.  sol.  in  KOH+ 
Aq;  very  stable  in  the  air.  (Melikoff  and 
Pissarjewsky,  Z.  anorg.  1899,  19.  408.) 

K4V2O12+2H2O.  (Melikoff  and  Pissar- 
jewsky, Z.  anorg.  1899,  19.  411.) 

K4V2Oi3+3^H2O.  Moderately  sol.  in 
H20  with  slow  decomp.  (Melikoff  and  Pissar- 
jewsky, Z.  anorg.  1899,  19.  410.) 

Silver  pervanadate,  AgVO4. 

SI.  sol.  in  H2O2+Aq  free  from  H2S04;  sol. 
in  alcohol.  (Scheuer.) 

Sodium  pervanadate,  NaVO4. 

Sol.  in  H2O-^  acidified  with  H2SO4;  insol. 
in  alcohol.  (Scheuer.) 

Strontium  pervanadate,  Sr(VO4)2. 

SI.  sol.  in  H2O2+Aq  free  from  H2SO4; 
insol.  in  alcohol.  (Scheuer.) 

Philippium,  Ph  (?). 

(Delafontaine,  C.  R.  87.  559.) 

Consists  of  terbium  and  yttrium.  (Roscoe, 
B.  15.  1274.) 

Phosgene,  CoCl2. 
See  Carbonyl  chloride. 

Phosphame,  PN2H  (?). 

Insol.  in  H2O.     Insol.  in  dil.  HNO3+Aq; 

gradually  decomp.  by  cone.  HNO3.     (Rose, 

Pogg.  24.  308.) 

Insol.  in  cone.  HNO3.    (Pauli,  A.  123.  236.) 
Sol.  in  H2SO4  with  decomp.    (Rose.) 
Insol.  in  dil.,  but  decomp.  by  cone.  KOH 

or  NaOH+Aq. 

Insol.  in  alcohol  or  ether. 

Formula  is  perhaps  P3N3H4.     (Sal/mann, 

B.  6.  494.) 

Phosphamic  acid,  PO<; 

\OH. 

(Schiff.) 

Does  not  exist,  but  was  impure  pyrophos- 
phodiamic  acid.  (Gladstone.)  Also  Mente 
(A.  248.  245). 


Pi/rophosphamic  acid,  P2NH3O6  = 
P2O3(OH)3NH2. 

Deliquescent  in  moist  air;  easily  sol.  in 
H2O  or  alcohol;  si.  sol.  in  ether.  (Gladstone, 
"hem.  Soc.  3.  152.) 

Correct  composition  is  imidocfo'phosphoric 

acid,  P2NH4O6  =  HO-™  ' 
(Mente,  A.  248.  232.) 


Barium  pyrophosphamate,  Ba3(P2NH2O6)2. 

Sol.  in  HC1  or  HNO3+Aq,  not  in  HC2H3O2 
,  Aq.     (Gladstone  and  Holmes,  Chem.  Soc. 
(2)  2.  233.) 


Cupric ,  C 

Ppt.    Decomp.  by  cold  KOH+Aq. 
stone,  Chem.  Soc.  3.  135.) 


(Glad- 


Ferric  ,  Fe2(P2NH2O6)2+2H2O. 

Insol.  in  dil.  acids.  Sol.  in  cone.  H2SO4, 
and  decomp.  by  warming.  Easily  sol.  in 
NH4OH+Aq.  Decomp.  by  KOH+Aq. 
(Gladstone,  Chem.  Soc.  3.  142.) 

Lead ,  Pb3(P2NH2O6)2-f  4H2O. 

Insol.  in  NH4OH+Aq. 

Potassium  -—,  K3P2NH2O6. 

Deliquescent.  Sol.  in  H2O.  Insol.  .in 
alcohol.  (Gladstone,  A.  76.  85.) 


Silver  - 
Ppt. 


-,  Ag3P2NH2O6+5H2O. 


Zinc ,  Zn3(P2NH2O6)2. 

(Gladstone  and  Holmes,  Chem.  Soc.  (2)  2. 

225.) 

Phosphamide,  PON. 
See  Phosphoryl  nitride. 
PN2H3O. 
See  Phosphoryl  imidoamide. 

jPnphosphamide,  PON2H6. 
See  Phosphoryl  iriamide. 

Tnwetaphosphimic  acid,  PsNsI^. 

Sol.  in  H2O;  aq.  solution  does  not  coagulate 
albumen.    (Stokes,  Am.  Ch.  J.  1895, 17.  275.) 

Ammonium  fn'wetaphosphimate, 

(NH4)3P3N306H3. 

Sol.  in  H2O,  insol.  in  alcohol;  unstable. 
(Stokes,  Am.  Ch.  J.  1896,  18.  643.) 

Barium  Jriwetaphosphimate,  Ba3(P3N3O6H3)2 

+4H20. 

+6H2O.     SI.  sol.  in  H2O.     Easily  sol.  in 
NH4Cl+Aq  and  in  NaCl+Aq.    (Stokes.) 


666 


PHOSPHIMATE,  BAREUM  SODIUM 


Barium  sodium  inwetaphosphimate, 

P3N3O6H3NaBa + 1  Jjli  »0 . 
Almost  insol.  in  H2O;  easily  sol.  in  NH4C1+ 
Aq  and  in  NaCl+Aq.    (Stokes.) 

Magnesium  Znwetaphosphimate, 

(P3N306H3)2Mg3  (?). 

Sol.  in  H2O;  insol.  in  alcohol;  aq.  solution 
decomp.  on  boiling.  (Stokes.) 

Potassium  ^nwetaphosphimate,  K3P3N3O6H3. 
Sol.  in  H2O;  insol.  in  alcohol.    (Stokes.) 

Silver  in'metophosphimate,  Ag3P3N3O6H3. 

Ppt.;  sol.  in  NH4OH+Aq;  insol.  in  H2O; 
si.  sol.  in  HNO3  + Aq.  (Stokes.) 

a  Sodium  Zn'wetaphosphimate,  P3N3O6H3Na3 

+4H20. 

18.3  pts.  are  sol.  in  100  pts.  H8O  at  20°; 
very  sol.  in  hot  H2O;  decomp.  by  alkali  on  long 
boiling.  (Stokes.) 

/3  Sodium  ^nwetaphosphimate,  P3N3O6H3Na3 

+H20. 
Sol.  in  H2O;  insol.  in  alcohol.    (Stokes.) 

TeJrawetaphosphimic  acid, 
P4N408H8+2H20. 

Very  si.  sol.  in  H2O;  decomposes  the  sol. 
salts  of  HC1,  H2SO4  and  HNO3.  (Stokes, 
Am.  Ch.  J.  1895,  17.  290.) 

100  pts.  H2O  at  20°  dissolve  0.64  pt.  crystal- 
lized acid.  Somewhat  more  sol.  in  boiling 
H2O.  (Stokes.) 

100  pts.  10%  HNO3+Aq  at  20°  dissolve 
0.26  pt.  of  crystallized  acid.  (Stokes.) 

Not  decomp.  by  boiling  alkalies +Aq. 
(Stokes,  Am.  Ch.  J.  1896,  18.  785.) 

Insol.  in  alcohol.  (Stokes,  Am.  Ch.  J. 
1896,  18.  784.) 

Ammonium  te£rametaphosphimate, 
P4N408H6(NH4)2. 

Only  si.  sol.  in  boiling  H2O;  sol.  in  excess 
ofhot5%HNO3.  (Stokes.) 

P4N4O8H4(NH4)4+4H2O.  Readily  sol.  in 
H2O;  si.  sol.  in  NH4OH+Aq.  (Stokes.) 

Barium  tefraraetaphosphimate,  P4N4O8H4Ba2 

+2H20. 
Ppt.;  insol.  in  H2O.    (Stokes.) 

Potassium  ^rametaphosphimate, 
P4N4O8H6K2. 

SI.  sol.  in  boiling  H2O;  sol.  in  cold  dil.  KOH 
+Aq.  (Stokes.) 

P4N4Q8H4K4  (?).  Very  sol.  in  H2O. 
(Stokes.) 

Silver  ^rametaphosphimate,  P4N4O8H4Ag4. 
Ppt.;  insol.  in  H2O;  si.  sol.  in  HNO8+Aq. 
(Stokes.) 


P4N4O8Ag8.     Ppt.;  sol.  in  NH4NO3+Aq. 

(Stokes.) 

Sodium  ^rawetaphosphimate,  P4N4O8H4Na4 


wetap 
?)  H20 


SI.  sol.  in  cold  H2O.  Easily  sol.  in  hot  H2O. 
Ppt.  from  aqueous  solution  by  excess  of  al- 
kali. (Stokes.) 

Penfometaphosphimic  acid, 

PO  ro™/NH-pa(OH)NH-PO(°H)\NH 
u-(-u±1\NH.PO.(OH)NH.PO(OH)/JN 

=  HioPsNsOio. 

Sol.  in  H2O;  pptd.  by  alcohol.  (Stokes,  Am. 
Ch.  J.  1898,  20.  748.) 

Magnesium  pentametaphosphimatej 
(P5N5010Hg)2Mg, 

Ppt.    (Stokes.) 

P5N6OioH6Mg2+5H2O.  Ppt.,  insol.  in  al- 
cohol; almost  insol.  in  H2O;  si.  sol.  in  cone. 
acetic  acid.  (Stokes.) 

Silver  pentaraetaphosphimate,  P5NsOioH6Ag5. 
Ppt.,  sol.  in  cold  KOH+Aq  with  decomp. 

(Stokes.) 

Sodium   pewtametaphosphimate, 

P5N5O10H5Na5+2H2O. 
Sol.  in  H2O;  insol.  in  alcohol.    (Stokes.) 
P5N5O10H6Na4+2H2O.    Sol.  in  80%  acetic 

acid;  pptd.  by  alcohol.    (Stokes.) 

Hexametaphosphiirdc  acid. 

Silver  Aezaraetaphosphimate,  PeNeO^HeAge. 

Ppt.;  decomp.  by  cold  KOH+Aq.  (Stokes, 
Am.  Ch.  J.  1898,  20.  757.) 


Sodium  hexametaphosphimaLte,  PeNe1 

+2H2O. 
Sol.  in  H2O;  pptd.  by  alcohol.    (Stokes.) 

Phosphine. 

See  Hydrogen  phosphide. 

PT/rophosphodiamic  acid, 

P2N2H60S  =  P203(OH)2(NH2)2. 

Deliquescent.  Easily  sol.  in  H2O,  alcohol, 
or  ether.  Sol.  in  cold  cone.  H2SO4  without 
decomp.  (Gladstone,  Chem.  Soc.  3.  353.) 

Correct  composition  is  cftimidodiphosphoric 
acid,  P2N2H404+H20  =HO— PO  =  (NH)2  = 
PO— OH.  (Mente.) 

Aluminum  pyrophosphodiaitLate. 

Precipitate.  Sol.  in  NH4OH+Aq.  Insol. 
in  acids.  (Gladstone,  A.  76.  82.) 

Ammonium ,  Psty^jj^' 

Very  deliquescent  in  moist  air.    Sol.  in  H2O. 


ery    equescen 
(Schiff,  A.  103.  168.) 


PHOSPBOARSENIOVANADICOVAN  ADIOTUN GSTATE,  AMMONIUM      667 


Barium  p^/rophosphocftamate, 

BaP2O6(NH2)2. 

Precipitate.  SI.  sol.  in  H2O.  Sol.  in 
NH4OH+Aq.  (Gladstone.) 

Calcium ,  CaP2O5(NH2)2. 

Insol.  in  NH4OH+Aq.  Sol.  in  NH4C1+ 
Aq  and  acids.  (Gladstone  and  Holmes.) 

Lead  — . 

Ppt.    Decomp.  by  H2O. 

Magnesium . 

Ppt.    (Gladstone  and  Holmes.) 

Silver ,  Ag2P2O5(NH2)2. 

SI.  sol.  in  H2O.  Sol.  inHNO3+Aq.  (Glad- 
stone and  Holmes.) 

Strontium . 

Sol.  in  acids  and  NH4Cl+Aq.  Insol.  in 
NH4OH+Aq.  (Gladstone  and  Holmes, 
Chem.  Soc.  (2)  4.  295.) 

Zinc ,  ZnP2O6(NH2)2. 

Ppt.    (Gladstone  and  Holmes.) 

Pyrophosphotriamic  acid,  P2N3H7O4  = 
OH 


Decomp.  by  boiling  H2O  or  HC1.  Sol.  in 
cone.  H2SO4  upon  heating.  (Gladstone  and 
Holmes.) 

Correct  formula  is.  HO—  PO< 

NH2  =diimidod^phosphoworiamic     acid. 
(Mente,  A.  248.  241.) 

Ammonium  pyrophosphotriamate, 


p  o       )4 

F2°3(NH2)3. 
Insol.  in  H2O.     (Gladstone  and  Holmes.) 

Barium  —  —  ,  BaP2N3H5O4. 

BaH2(P2N3H5O4)2.  Decomp.  by  HCl+Aq. 
(Gladstone,  Chem.  Soc.  4.  6.) 

Cobaltous  ---  ,  CoP2N3H5O4. 

Slowly  decomp.  by  dil.  H2SO4+Aq,  not  by 
HCl+Aq.  (Gladstone  and  Holmes,  Chem. 
Soc.  (2)  4.  1.) 

Cupric  -  ,  CuP2N3H5O4. 

Insol.  in  H2O  or  NH4OH  +  Aq.  (Gladstone 
and  Holmes,  Chem.  Soc.  (2)  4.  1.) 

Ferrous  --  ,  FeH6(P2N3H3O4)2.   ' 

Insol.  in  dil.  acids.  (Gladstone,  Chem.  Soc. 
(2)  4.  1.) 

Lead  --  ,  H2Pb3(P2N3H3O4)2. 

Ppt.  (Gladstone  and  Holmes,  Chem.  Soc. 
(2)  4.  1.) 


H4Pb2(T2N3H3O4)2.    Ppt.    (G.  and  H.) 
H6Pb(P2N3H3O4)2.    (G.  and  H.) 

Mercuric  pyrophosphotriamate, 

Hg2P2N3H304. 

Insol.  in  H2O  or  dil.  HC1  or  HNO3+Aq. 
(Gladstone  and  Holmes,  Chem.  Soc.  (2)  4.  1.) 

Platinum ,  Pt2P2N3H3O4. 

Decomp.  by  H2O  when  freshly  pptd.  (G. 
and  H.) 

Potassium ,  KP,N3H6O4. 

Almost  insol.  in  H2O.  (Gladstone,  Chem. 
Soc.  4.  10.) 

Silver ,  Ag3P2N3H4O4. 

Ppt.  SI.  attacked  by  HC2H3O2;  decomp. 
by  HNO3  or  NH4OH+Aq  into— 

AgH2P2N3H4O4.  Insol.  in  H2O.  Decomp. 
by  HC1.  (Gladstone,  Chem.  Soc.  (2)  4.  1.) 

Zinc . 

Insol.  in  H2O.    (Gladstone  and  Holmes.) 

JWraphosphocframic  acid,  P4N2H8Oii  = 


P407 


(OH), 
(NH2)2. 


Known  only  as  NH4  salt. 

Ammonium  tetraphosphodiamate, 
04H(NH4)3 


^ 
Very  deliquescent,  and  sol.  in  H2O.    (Glad- 

stone.) 

Ammonium  ^hydrogen  te^raphosphocfo'amate, 


:etraphosph( 

4H2(NH4)2 


Insol.  in  cold,  easily  sol.  in  hot  H2O  and  dil. 
acids.    (Gladstone.) 

Tetraphosphotetramic  acid, 


Sol.  in  H2O.    Insol.  in  alcohol.   (Gladstone.) 

Ammonium  tetraphosphot  etramate, 

p  0  (02HNH4) 

P4°7(NH2)4. 

Sel.  in  H2O,  and  precipitated  from  solution 
by  alcohol.    (Gladstone.) 

Silver  --  ,  Ag6P4N4H4O9. 
Ppt. 

Ag2H4P4N4H409.    Ppt. 

Ammonium       phosphoarseniovanadico- 
vanadiotungstate. 

See    Arseniophosphovanadicovanadiotung- 
state,  ammonium. 


668 


PHOSPHOAZOTIC  ACID 


Tetraphosphopentsizotic  acid, 


Ins  pi.  in  H2O.    Decomp.  gradually  by  boil- 
ing with  H/).    (Gladstone.) 

Ammoniotetraphosiphopentazotic  acid  (?), 


Decomp.  by  H2O.    (Gladstone.) 

Cupric  tetraphosphopentazot&te, 

(Gladstone,  Chem.  Soc.  (2)  6.  261.) 

Lead^ . 

(Gladstone,  Chem.  Soc.  (2)  6.  261.) 

Potassium ,  KOP4N5H806. 

Insol.  in  HoO.  (Gladstone,  Chem.  Soc.  (2) 
6.  268.) 

Phosphoboric  acid,  H3BO3,  H3PO4  =  BPO4 

+3H2O. 

Not  decomp.  by  boiling  H2O  or  cone,  acids. 
Sol.  in  boiling  solution  of  caustic  alkalies. 
(Vogel,  N.  Repert.  Pharm.  18.  611.) 

Phosphochloroplatinous  acid, 

P(OH)3,  PtCl2. 
See  Chloroplatinophosphoric  acid. 

Phosphochromic  acid. 

Ammonium  phosphochromate,  3(NH4)2O, 

P2O5,  8CrO3+H2O. 

Sol.  in  H2O  with  decomp.  (Friedheim,  Z. 
anorg.  1894,  6.  284.) 

Potassium  phosphochromate,  2K2O,  P2O5, 
4CrO3+H2O. 

Sol.  in  H2O  but  cannot  be  cryst.  therefrom 
without  decomp.  Can  be  cryst.  without  de- 
comp. from  H2O  containing  phosphoric  acid. 
(Friedheim.) 

3K2O,  P2O6,  8CrO3.  Sol.  in  H2O  but 
cannot  be  cryst.  therefrom  without  decomp. 
(Blondel,  C.  R.  1894,  118.  194.) 

Phosphohypophosphotungstic  acid. 

Potassium  sodium  phosphohypophosphotung- 
state,  9K2O,  Na2O,  4P2O5,  2PO2H3, 
26WO3+23H2O. 

Precipitate.  Easily  sol.  in  hot  H2O. 
(Gibbs,  Am.  Ch.  J.  7.  313.) 

Tetraphosphotetrimidic  acid, 


Known  only  in  its  salts.    (Gladstone.) 


Silver  ^raphosphote£rimidate. 
Ppt.    (Gladstone.) 

Phosphoiodic  acid,  P2O5,  18I2O5+4H2O. 

Decomp.  by  H2O.  (Chretien,  A.  ch.  1898, 
(7)  15.  389.) 

Ammonium  phosphoiodate,  4(NH4)2O,  P2O5, 

18I2O5  +  12H2O. 

Sol.  in  H2O.  SI.  sol.  in  cone.  H3PO4+Aq. 
(Chretien.) 

Lithium  phosphoiodate,  3Li2O,  P2O5,  18I2O5  + 

11H2O. 
Sol.  in  H2O.    SI.  sol.  in  cone.  H3PO4+Aq. 

(Chretien.) 

Potassium  phosphoiodate,  4K2O,  P2O5, 

18I2O5+5H2O. 

Decomp.  by  a  small  amt.  of  H2O;  sol.  in  a 
large  amt.  SI.  sol.  in  cone.  H3PO4+Aq. 
(Chretien.) 

Sodium  phosphoiodate,  6Na2O,  P2O5,  18I2O5 

+5H20. 
Sol.  in  H2O.    SI.  sol.  in  cone.  H3PO4+Aq. 

(Chretien.) 

Phosphoiridic  acid. 

See  Chlorophosphoiridic  acid. 

Phospholuteotungstic  acid,  H5PW8O29. 
See  under  Phosphotungstic  acid. 

Phosphomolybdic  acid,  P2O6,  18MoO3 


11  Phospholuteomolybdic  acid." 

Deliquescent.  Sol.  in  H2O  in  all  propor- 
tions. (Kehrmann,  Z.  anorg.  1894,  7.  418.) 

3H2O,  P2O5,  20MoO3+21H2O.  Very  sol. 
in  H2O.  Sol.  in  ether.  By  evaporation  of 
H2O  solution  crystals  with  44H2O,  or  from 
a  strong  solution  in  cone.  HNO3+Aq,  with 
19H2O,  are  obtained;  also  crystals  with  38, 
and  48H2O  are  known.  (Debrav,  C.  R.  66. 
704.) 

According  to  Rammelsberg  (B.  10.  1776) 
formula  is  3H2O,  P2O5,  22MoO3. 

According  to  Gibbs  (Am.  Ch.  J.  3.  317) 
formula  is  3H2O,  P2O5,  24MoO3+59H2O. 

Finkener  (B.  11.  1638)  gives  the  formula  as 
3H2O,  P2O5,  24MoO3+58H2O,  also  with 
29H20. 

P2O5,  20MoO3+52H2O.  Sol.  in  dry  ether 
with  evolution  of  heat,  and  subsequent  separ- 
ation into  two  layers,  the  upper  consisting  of 
pure  ether,  and  lower  of  a  solution  of  acid  in 
ether.  Sp.  gr.  of  lower  layer,  when  sat.  at 
13°,  is  1.3.  On  warming  lower  layer,  ether 
separates  out  and  forms  an  upper  layer.  This 
redissolves  on  cooling  and  shaking.  The  lower 
layer  is  insol.  in  H2O  and  miscible  with  al- 
cohol. 


PHOSPHOMOLYBDATE,  AMMONIUM  CADMIUM 


669 


100  pts.  ether  thus  dissolve  80.6  pts.  acid 
at  0°;  84.7  pts.  at  8.1°;  96.7  pts.  at  19.3°; 
103.9  pts.  at  27.4°;  107.9  pts.  at  32.9°.  (Par- 
mentier,  C.  R.  104.  688.) 

P2O5,  22MoO3+57H2O,  and  +58H2O. 
(Pohl,  Dissert.  1906.) 

P2O5,  23MoO3+61H20.    (Pohl.) 

P2O5,  24MoO3+61H2O.  (Miolati,  C.  C. 
1903,  11.  789.) 

+64H2O.    (Pohl.) 

Diphosphope/itomolybdic  acid, 

H6P2Mo5O23  =  3H2O,  P2O5,  5MoO3. 
Not  known  in  free  state. 

Ammonium  phosphomolybdate,  (NH4)2O, 
P2O5,  2MoO8+2H2O. 

(Meschorier,  Dissert.  1894.) 

2(NH4)2O,  P2O6,  4MoO3+5H2O.  (Fried- 
heim,  Z.  anorg.  1894,  6.  33.) 

+6H2O.    (Perlberger,  Dissert.  1904.) 

(NH4)3PO4,  HMo03+6H2O. 

Formula  is  (NH4)3PO4,  10MpO3  +  l^H2O, 
according  to  the  older  authorities. 

Scarcely  sol.  in  H2O  or  aqueous  acid  solu- 
tions. Easily  sol.  in  ammonia,  and  alkalies + 
Aq.  (Svanberg  and  Struve,  J.  pr.  44.  291.) 

It  is  almost  completely  insol.  in  a  mixture 
of  CNH4)2MoO4+Aq,  and  dil.  HNO3+Aq. 
Absolutely  insol.  in  a  dil.  nitric  acid  solution 
of  ammonium  nitrate.  (Richters,  Z.  anal.  10. 
471.) 

Solubility  is  increased  even  in  presence  of 
ammonium  molybdate  and  free  HNO3  by 
HC1,  ammonium,  and  other  chlorides,  tar- 
taric  acid,  or  large  quantities  of  ammonium 
oxalate  or  citrate.  Not  precipitated  in  pres- 
ence of  excess  of  H3PO4.  (Fresenius,  Z.  anal. 
3.  446.) 

Sol.  in  10,000  pts.  H2O  at  16°;  in  6600  pts. 
H2O  containing  1  vol.  %  HNO3;  in  550  pts. 
HCl+Aq  of  1.12  sp.  gr.;  in  620  pts.  alcohol 
of  0.80  sp.  gr.;  in  190  pts.  HNO3+Aq  (sp. 
gr.  - 1.2)  at  50°;  in  5  pts.  cone.  H2SO4  at  100°; 
in  3  pts.  NH4OH+Aq  of  0.95  sp.  gr.  (Eggertz, 
J.  pr.  79.  496.) 

Sol.  in  21,186  pts.  H2O,  38,117  pts.  dil. 
alcohol,  and  13,513  pts.  strong  alcohol. 
(Hehner,  Analyst,  1879.  23.) 

According  to  Sonnenschein,  the  solubility  is 
increased  by  much  H2O  or  alcohol,  alkaline 
hydroxides,  carbonates,  ortho-,  pyro-,  and 
metaphosphates;  sodium  borate,  hyposul- 
phate,  thiosulphate,  acetate,  arsenate,  and 
arsenite;  potassium  sodium  tartrate,  ammo- 
nium oxalate,  orthophosphoric  acid,  and  sul- 
phuric acid.  It  is  not  increased  by  ammo- 
nium molybdate  or  sulphate,  potassium  sul- 
phate, acid  tartrate,  acid  oxalate,  nitrate,  or 
chlorate,  iodide,  chloride,  or  bromide;  sodium 
bromide  or  nitrate;  nitric,  hydrochloric,  boric, 
tartaric,  oxalic,  and  dilute  sulphuric  acids. 
(Sonnenschein,  J.  pr.  63.  342.) 

Sol.  in  hot  H2O.  Sol.  in  cold  caustic 
alkalies,  alkali  carbonates,  and  phosphates, 


NH4C1,  and  (NH4)2C2O4+Aq;  si.  sol.  in 
(NH4)2SO4,  KNO3,  and  KCl+Aq;  very  si.  sol. 
in  NH4NO3+Aq.  Sol.  in  K2SO4,  Na2SO4, 
NaCl,  MgCl2,  H2SO4,  HC1,  and  cone,  or  dil. 
HNO3+Aq. 

Presence  of  (]\H4)2MoO4  totally  changes 
the  effect  of  acid  liquids;  insol.  in  dil.  HNO3  or 
H2SO4+Aq  containing  (NH4)2MoO4,  but 
somewhat  sol.  in  HCl+Aq,  even  in  presence 
of  that  salt.  Tartaric  acid  and  similar  organic 
substances  totally  prevent  the  precipitation 
of  this  salt.  (Eggertz  in  Fresenius'  Quant, 
anal.) 

5(NH4)2O,  48MoO3,  2P2O6  +  17H2O  = 
3(NH4)2O,  24MoO3,  P2O5+2(NH4)2O,  H2O, 
24MoO3,  P2O5+16H2O.  Formula  of  above 
salt  according  to  Gibbs. 

3(NH4)2O,    22MoO3,    PoO5+9H2O,    or 
12H20. 

8(NH4)2O,  H2O,  60MoO3,  3P2O5+11H2O. 
SI.  sol.  in  H2O. 

3(NH4)2O,  16MoO3,  P2Oft+14H2O.  Insol. 
in  cold,  sol.  with  decomp.  in  hot  H2O.  Sol. 
in  NH4OH+Aq.  (Gibbs,  Am.  Ch.  J.  3.  317.) 

5(NH4)oO,  P2O5,  16MoO3.  (Meschoirer, 
Dissert,  1894.) 

3(NH4)2O,  P2O5,  18MoO3+14H2O.  Sol. 
in  H2O.  The  aqueous  solution  is  stable  at 
ordinary  temp,  for  several  days,  but  when 
warmed  ordinary  ammonium  phosphomolyb- 
date separates.  (Kehrmann,  Z.  anorg.  1894, 
7.  414.) 

3(NH4)2O,  P2O5,  28MoO3+8H2O.  100  g. 
H2O  dissolve  0.0238  g.  at  15°.  1  pt.  is  sol.  at 
15°  in  4206  pts.  H2O;  7300  pts.  5%  NH4N08+ 
Aq;  4930  pts.  1%  HNO3+Aq.  (de  Lucchi, 
Rass.  Min.  1910,  32.  21.) 

9(NH4)2O,  2P2O5,  28MoO3+8H2O.  (Mes- 
choirer, Dissert.  1894.) 

Ammonium  eftphosphopentamolybdate, 

2(NH4)3PO4,  5MoO3+7H,O  =  3(NH4)2O, 
5MoO3,  P2O5+7H2O. 

Easily  sol.  in  hot,  less  in  cold  H2O.  (Zenk- 
ner,  J.  pr.  58.  256.) 

5(NH4)2O,  H2O.  10MoO3,  2P2O5+6H2O 
=  3(NH4)2O,  5MoO3,  P2O5+2(NH4)2O,  H2O, 
5MoO3,  P2O5+6H2O.  Sol.  in  H,O.  (Gibbs, 
Am.  Ch.  J.  1895,  17.  87.) 

+8H,O.    (Perlberger.) 

+  18H2O.  (Mazzuchelli  and  Zangrilli, 
Gazz.  ch.  it.  1910,  40.  (2)  55.) 

5(NH4)2O,  P206,  10MoO8+13H2O,  and 
+14H2O.  (Perlberger,  Dissert.  1904.) 

Ammonium  barium  phosphomolybdate, 
3(NH4)2O,  30BaO,  P2O5,  30MoO3. 
Insol.  precipitate.     (Seligsohn,  J.  pr.  67. 

478.) 

Ammonium   cadmium   phosphomolybdate, 
5(NH4)2O,  CdO,  P2O5,  6MoO3+8H2O. 

(Perlberger,  Dissert,  1904.) 

3(NH4)2,  2CdO,  2P2O6,  9MoO3-f  141H2O. 
(Perlberger.) 


670 


PHOSPHOMOLYBDATE,  AMMONIUM  COBALTOUS 


Ammonium  cobaltous  phosphomolybdate, 
(NH4)2O,  2CoO,  P2O8,  5MoO3  +  10H2O. 

Decomp.  by  cold  H2O.  Sol.  in  acids  and 
hot  H2O.  (Arnfeld,  Dissert,  1898.) 

4(NH4)26,  CoO,  2P2O5,  10MoO3  +  12H2O. 
SI.  sol.  in  cold,  easily  sol.  in  hot  H2O.  (Arn- 
feld.) , 

Ammonium  manganous  phosphomolybdate, 
(NH4)2O,  2MnO,  P2O5,  5MoO3+20H2O. 

Decomp.  by  H2O,  but  dissolves  clear  on 
heating.  (Arnfeld.) 

4(NH4)2O,  MnO,  2P2O5,  10MoO3  +  13H2O. 
(Arnfeld.) 

5(NH4)2O,  IGMnO,  2P2O5,  20MoO3  + 
10H2O.  Very  si.  sol.  in  H2O.  (Gibbs,  Am. 
Ch.  J.  1895,  17.  87.) 

Ammonium    nickel    phosphomolybdate, 

(NH4)2O,  2NiO,  P2O5,  5MoO3  +  10H2O. 

Decomp.  by  cold,  but  sol.  in  hot  H2O. 
(Arnfeld.) 

(NH4)2O,  NiO,  2P2O5,  10MoO8  +  12H2O. 
Very  sol.  in  H2O.  '  (Arnfeld.) 

Ammonium    potassium     phosphomolybdate, 
6(NH4)2O,     15K2O,    2P2O5,    60MoO3  + 
12H20. 
Sol.  in  H2O.    Insol.  in  alcohol.    (Seligsohn, 

J.  pr.  67.  477.) 

Ammonium  sodium  phosphomolybdate, 

6(NH4),O,    15Na2O,    2P2O5,    60MoO3  + 
18H2O. 

Sol.  in  much  boiling  H2O.  Insol.  in  alcohol. 
(Seligsohn,  J.  pr.  67.  474.) 

Barium     phosphomolybdate,     3BaO,     P2O5, 

24MoO3+zH2O. 

Moderately  sol.  in  cold,  very  easily  sol.  in 
hot  H2O.  Decomp.  in  aqueous  solution  at 
ordinary  temp,  on  standing.  (Kehrmann, 
Z.  anorg.  1894,  7.  414.) 

Cgssium    phosphomolybdate,    3Cs2O,^P2O5, 

6MoO3-H8H2O. 

Ppt.    (Ephraim,  Z.  anorg.  1910,  65.  240.) 
2Cs2O,  P2O5,  14MoO3+3H2O.     Difficultly 

sol.  in  H2O.    (Ephraim.) 

3Cs2O,    P265,    21MoO3+4H2O    (?). 

(Ephraim.) 

Calcium  potassium  phosphomolybdate,  2CaO, 

3K2O,  2P2O5,  10MoO3+22H2O. 
(Friedheim,  Z.  anorg.  1893,  4.  293.) 

Cobaltous  phosphomolybdate,  2CoO,  P2O5, 
4MoO3+zH2O. 

(Arnfeld,  Dissert.  1898.) 

3CoO,  P2O5,  5MoO3  +  16MH2O,  and  +  17K 
H2O.  Extremely  sol.  in  H2O.  (Arnfeld.) 

3CoO,  P2O5,  18MoO3+38H2O.  Sol.  in 
H2O.  (Arnfeld.) 

3CoO,  P2O6,  24MoO3-|-58H2O,  and+60H2O. 
Sol.  in  HoO.  (Arnfeld.) 


Cobaltous  potassium  phosphomolybdate, 

K2O,  2CoO,  P2O5,   5MoO3+15H2O. 
(Arnfeld.) 

4K2O,  CoO,  2P2O5,  10MoO3  +  12H2O.  SI. 
sol.  in  cold,  easily  sol.  in  hot  H20.  (Arnfeld.) 

Croceocobaltic  phosphomolybdate,  24MoO3, 
P205,     [Co(NH3)4(N02)2]20,    2H20  + 
21H2O. 
SI.  sol.  in  cold,  easily  in  hot  H2O.    (Gibbs, 

Am.  Ch.  J.  3.  317.) 

Gold  phosphomolybdate  ammonia,  12Au2O3, 

7P2O0,  3MoO3,  24NH3+21H2O. 
Insol.  in  H2O.     (Gibbs,  Am.  Ch.  J.  1895, 
17.  172.) 

Gold   sodium   phosphomolybdate   ammonia, 
5Au2O3,  Na2O,  P2O5,  HMoO3,  15NH3  + 
10H2O. 
Sol.  in  dil.  HC1.    Almost  insol.  in  NH4OH  + 

Aq.    (Gibbs.) 

Lead  phosphomolybdate,  23PbMo04,   P2O5, 

2PbPO4+7H2O. 

Sol.  in  500,000  pts.  H2O.  Insol.  in  NH4OH 
+Aq.  Easily  sol.  in  KOH,  ISlaOH,  or  HNO3 
4-Aq;  somewhat  less  sol.  in  HC2H3O2-fAq. 
(Beuf,  Bull.  Soc.  (3)  3.  852.) 

Lithium  phosphomolybdate,   12Li2O,   4P2O5, 

5MoO3  +  18H2O. 
Partially  sol.  in  H2O.    (Ephraim,  Z.  anorg. 

1909,  64.  233.) 
3Li2O,  P2O5,  5MoO3  +  16H2O.    Ppt. 

(Ephraim,  Z.  anorg.  1910,  65.  233-6.) 
3Li2O,  P2O5,  5MoO3  +  17H2O.    Ppt.    (E.) 
5Li2O,  2P2O5,  8MoO3+28H2O.    Easily  sol. 

in  H2O.    (E.) 

3Li2O,  P2O5,  12MoO3  +  18H2O.    Ppt.    (E.) 
3Li2O,    P2O5,    18MoO3+27H2O.      Sol.    in 

H2O.    (E.) 

Manganous  phosphomolybdate,  3MnO,  P2O5, 
5MoO3+20H2O. 

Very  sol.  in  H2O.  SI.  sol.  in  alcohol.  (Arn- 
feld.) 

3MnO,  P2O5,  18MoO3+38H2O.  Sol.  in 
H2O.  (Arnfeld.) 

3MnO,  P2O5,  24MoO3+58H2O,  and +60 
H2O.  Easily  sol.  in  H2O.  (Arnfeld.) 

Manganous    potassium    phosphomolybdate, 

2MnO,  3K2O,  2P2O5,  10MoO3+30H2O. 
Sol.  in  hot  H2O.    (Arnfeld.) 

Manganous  sodium  phosphomolybdate, 

7MnO,  9Na2O,  2P2O5,  22MoO3+57H2O. 

Nearly  insol.  in  cold  H2O.  Sol.  in  boiling 
H2O  but  decomp.  thereby.  (Gibbs,  Am.  Ch. 
J.  1895,  17.  85.) 

Nickel   phosphomolybdate,   2NiO,    P-..O5, 
4MoO3+zH2O. 

Ppt.    (Arnfeld.) 

3NiO,  P2O5,  5MoO3+20H2O.  Decomp.  by 
H2O.  '(Arnfeld.) 


PHOSPHONITRYLATE,  SILVEB 


671 


3NiO,  P2O5,  18MoO3-t-34H2O.  Sol.  in 
H,O.  (Arnfeld.) 

3NiO,  P2O5,  24MoO3+58H2O,  and+60H2O. 
Efflorescent.  Sol.  in  H2O.  (Arnfeld.) 

Nickel  potassium  phosphomolybdate,  K2O. 
2NiO,  P2O5,  5MoO3  +  13H2O. 

Decomp.  by  cold  H2O,  but  goes  into  solu- 
tion by  boiling.  (Arnfeld.) 

4K2O,  NiO,  2P2O5,  10MoO3  +  12H2O.  Sol. 
in  H2O.  (Arnfeld.) 

Potassium    phosphomolybdate,    K3PO4, 

HMoO3  +  l^H2O  =3K2O,  P2O5, 22MoO3 
+3H2O. 

Insol.  in  H2O.  Easily  sol.  in  alkalies. 
(Svanberg  and  Struve.) 

100  g.  H2O  dissolve  0.007  g.  at  30°;  100  g. 
10%  HNOa+Aq  dissolve  0.204  g.  at  30°. 
(Donk,  Bull.  90,  Bur.  of  Chem.,  U.  S.  Dept. 
of  Agric.  1905.) 

According  to  older  authorities  the  formula 
is  K3PO4,  10MoO3  +  l^H2O. 

-f6H2O.    (Rammelsberg.) 

2K2O,  H2O,  24MoO3,  P2O5+3H,O.  SI.  sol. 
in  cold  H2O. 

5K2O,  H2O,  44MoO3,  2P2O5+21H,O. 
(Gibbs,  Am.  Ch.  J.  3.  317.) 

3K2O,  P2O6, 18MoO3+llH2O,  and  +15H2O 
(EUas.) 

+  14H2O.  SI.  sol.  in  cold,  very  easily  sol. 
in  hot  H2O.  Can  be  cryst.  from  hot  H2O. 
(Kehrmann,  Z.  anorg.  1894,  7.  416.) 

3K2O,  P2O5,  17MoO3  +  12H2O.  Moder- 
ately sol.  in  H2O.  (Elias,  Dissert.  1906.) 

5K2O,  P2O6,  17MoO3+zH2O.  Aqueous 
solution  decomp.  rapidly  in  the  cold.  (Kehr- 
mann, Z.  anorg.  1894,  7.  423.) 

4K2O,  2H2O,  9MoO3,  P2O5  +  18H2O. 
(Zenkner.) 

5K2O,  H,O,  10MoO3,  P2O5  +  19H2O.  Eas- 
ily sol.  in  H2O.  (Rammelsberg,  B.  10.  1776.) 

6K2O,  15MoO3,  P2O5.  Insol.  in  H2O.  Sol. 
inKOH+Aq.  (Rammelsberg.) 

K2O,  P2O5,  2MoO3  +  13H26.  Very  sol.  in 
H2O.  (Friedheim,  Z.  anorg.  4.  287.) 

2K2O,  P2O5,  4MoO3+8H2O.  Sol.  in  H2O. 
(Friedheim.) 

Potassium  diphosphopentamolybdate,  3K2O, 
P2O5,  5MoO3+7H2O. 

Sol.  in  H2O;  precipitated  by  HNO3  or  HC1 
+Aq.  (Zenkner,  J.  pr.  68.  261.) 

2K2O,  P2O5,  5MoO3+6H2O.    (Friedheim.) 

Potassium  cfo'phosphopentamolybdate  nitrate, 

2K3PO4,  5MoO3,  6KNO3+9H2O. 
(Debray,  C.  R.  66.  706.) 

Rubidium  phosphomolybdates: 

7Rb2O,  P2O5,  22MoO3+12H2O;  3Rb2O, 
P205, 20MoO3  +  12H2O;  6RboO,;P2O5, 18MoO3 
+  10H.O;  5Rb2O,  2P2O6,  9MoO3  +  13H2O; 
7Rb2O,  3P2O5,  10Mo08  +  15H2O.  (Ephraim, 
Z.  anorg.  1910,  65.  237-9.) 


Silver  phosphomolybdate,  7Ag2O,  P2O5, 
20MoO3+24H2O. 

Ppt.    Sol.  in  dil.  HNO3+Aq,  forming— 

2Ag2O,  P2O5,  20MoO3+7H2O.  SI.  sol.  in 
H2O.  (Rammelsberg.) 

Formula  of  first  salt  is — 

7Ag2O,  22MoO3,  P2O5  +  14H2O.  Sol.  in  hot 
H2O,  but  solution  is  quickly  decomp.  (Gibbs, 
Am.  Ch.  J.  3.  317.) 

7Ag2O,  P2O5,  24MoO3.  Ppt.  (Miolati,  J. 
pr.  1908  (2)  77.  451.) 

Silver  cftphosphopentamolybdate, 

Ag6Mo5P2O23+7H2O. 
Easily  sol.  in  H2O.    (Debray,  C.  R,  66.  705.) 

Sodium  phosphomolybdate. 

Sol.  in  H2O  and  HNO3+Aq.  (Sonnen- 
schein,  A.  104.  45.) 

Na2O,  5HoO,  P2O6,  18MoO3+xH2O. 

2Na2O,  4H2O,  P2O5,  18MoO3+xH2O. 

3Na2O,  P2O5,  18MoO3+26H2O.  (Fried- 
heim.) 

3Na2O,  P2O5,  24MoO3+42H2O.  (Rosen- 
heim  and  Pinsker,  Z.  anorg.  1911,  70.  79.) 

Sodium    diphosphopentomolybdate,     3Na2O, 

P2O5,  5MoO3+14H2O. 
Easily  sol.  in  H2O.    (Debray.) 

Sodium  auramine  phosphomolybdate,  Na2O, 

5Au2O3,  2P2O5,   HMoO,,   15NH3. 
Sol.  in  hot  H2O.    Very  sol.  in  hot  HC1. 
(Gibbs,  Am.  Ch.  J.  1895,  17.171.) 

Metaphosphomolybdic  acid. 

Ammonium    mono wetaphosphomolyb date, 
3(NH4)2O,  4NH4PO3,  10MoO3+9H2O. 
Very  sol.  in  H2O.     (Gibbs,  Am.  Ch.  J.  7. 
392.) 

Barium     Aezcmetaphosphomolybdate,     BaO, 

Ba3(PO3)6,  14MoO3+55H2O. 
Sol.  inH2O.    (Gibbs.) 

PwrophosphonitryUc  acid,  P,HNO4  = 
OH 


P,O; 


N. 


Not  known  in  free  state. 

Ammonium  pyrophosphonitrylate, 
0  ONH4 
2    3N. 

Insol.    but    gradually    decomp.    by    H2O. 
(Gladstone.) 

Potassium  —  — ,  KP2NO4. 
Insol.  in  H2O.    (Gladstone.) 

Silver ,  AgP2NO4. 

Ppt. 


672 


PHOSPHONITRILIC  CHLORAMIDE 


TYiphosphonitrilic  chloramide, 

P3N3C14(NH2)2. 

Sol.  in  H2O  without  decomp.;  sol.  in  ether, 
alcohol;  si.  sol.  in  benzene.  (Stokes,  Am.  Ch. 
J.  1895,  17.  287.) 

TViphosphonitrilic  tefrachlorhydrin, 

P3N3C14O2H2. 

Sol.  in  ether,  alcohol,  and  H2O;  insol.  in 
benzene  and  CS2.  (Stokes,  Am.  Ch.  J.  1895, 
17.  286.) 

Tn'phosphonitrilic  chloride,  P3N3C16. 

Sol.  in  glacial  acetic  acid  and  H2SO4.  100 
pts.  ether  dissolve  46.5  pts.  at  20°.  (Liebig.) 

Insol.  in  light  petroleum;  sol.  in  benzene. 
(Stokes,  Am.  Ch.  J.  1897,  19.  783.) 

TWraphosphonitrilic  chloride,  P4N4C18. 

Sol.  in  alcohol,  ether,  benzene,  H2SO4.  SI. 
sol.  in  H2O  with  decomp.  100  pts.  ether  dis- 
solve 12.3  pts.  at  20°.  (Stokes,  Am.  Ch.  J. 
1895,  17.  281.) 

Pentaphosphonitrilic     chloride,     (PNC12)5  = 

P5N5C110. 

Sol.  'in  benzene,  light  petroleum,  acetic 
acid,  ether,  CS2;  insol.  in  H2O.  (Stokes,  Am. 
Ch.  J.  1897,  19.  790.) 

flerraphosphonitrilic  chloride,  (PNC12)6  = 

P6N6C112. 

Sol.  in  benzene,  light  petroleum,  ether, 
CS2;  insol.  in  H2O.  (Stokes.) 


JF/eptaphosphonitrilic 
P7N7C114. 


chloride,     (PNC12)7  = 


Sol.  in    benzene,    light  petroleum,  ether, 
CS2;  insol.  in  H2O;  sol.  in  alcohol  with  decomp. 

(Stokes.) 

Pofo/phosphonitrilic  chloride,  (PNCl2)a;. 

Depolymerizes  on  distillation;  insol.  in 
benzene  and  light  petroleum  and  all  neutral 
solvents;  sol.  in  H2O  with  decomp.  (Stokes.) 

Phosphonitrilochloramide,  P2N2C13(NH2) . 

Slowly  sol.  in  H2O  with  decomp.  Insol. 
in  ether  and  CSo.  SI.  sol.  in  boiling  CC14. 
(Besson  and  Rosset,  C.  R.  1908,  146.  1149.) 

Phosphonium  bromide,  PH4Br. 

Decomp.  violently  by  H2O. 

Phosphonium  chloride,  PH4C1. 
(Ogier,  Bull.  Soc.  (2)  32.  483.) 

Phosphonium    titanium    chloride,    2PH4C1, 

3TiCl4. 

Decomp.  by  H2O,  HC1,  or  alkalies  +Aq. 
R  ose.) 


Phosphonium  iodide,  PH4I. 

Decomp.  by  H2O,  alkalies,  alcohol,  etc. 
(Rose,  Pogg.  46.  636.) 

Decomp.  by  PC13.    (Wilde,  B.  16.  217.) 

Phosphonium  sulphate  (?).    . 

Deliquescent;  very  unstable.  (Besson, 
C.  R.  109.  644.) 

Phosphoramide,  P(NH2)3. 

Insol.  in  NH4Br,  3NH3;  sol.  in  NHJ,  3NH3. 
(Hugot,  C.  R.  1905,  141.  1235.) 

Phosphortn'amide,  PON3H6. 

See  Phosphoryl  in'amide. 
Phosphoric  acid,  anhydrous,  P2Os. 

See  Phosphorus  pentoxide. 
Afetaphosphoric  acid,  HPO3. 

Sol.  in  H2O.  Not  isolated.  (Fleitmann, 
Pogg.  78.  362.) 

Deliquescent.  Sol.  in  H2O,  but  aqueous 
solution  decomp.  into  H3PO4,  slowly  in  the 
cold,  but  more  rapidly  on  heating.  Cone, 
solutions  decomp.  more  rapidly  than  when 
dil.  (Giran,  A.  ch.  1903,  (7)  3(f.  203.) 

Insol.  in  liquid  CO2.  (Biichner,  Z.  phys. 
Ch.  1906,  54.  674.) 

ZH'raetaphosphoric  acid,  H2P2O6. 

Not  isolated.    (Fleitmann.) 

Tnmetaphosphonc  acid,  H3P3O9. 

Sol.  in  H2O;  the  solution  is  permanent  in 
the  cold,  but  on  evaporation  it  is  quickly  de- 
comp. to  H3PO4. 

Tetrametaphosphonc  acid,  H4P4Oi2. 
Not  isolated. 

Hexametaphosphoric  acid,  H6P6Oi8. 
(Glacial  phosphoric  acid.) 

Deliquescent;  easily  sol.  in  H2O  with  evolu- 
tion of  heat  and  conversion  into  H3PO4.  Not 
easily  sol.  in  presence  of  slight  impurities. 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 

Or#w>phosphoric  acid,  H3PO4. 

Very  sol.  in  H2O. 

100  pts.  of  the  solution  contain  at: 
26.23°      27.02°      29.42°      29.77° 
95.9         95.98        96.15        96.11  pts.  H3PO4, 

37.65°       39.35°      42.30°  (mpt.) 
97.8          98.48         100  pts.  H3PO4. 
(Smith  and  Menzies,  J.  Am.  Chem.  Soc.  1909, 
31.  1186.) 

See  also  10H3PO4+H2O,  and  2H3P04+ 
H2O. 

Sp.  gr.  of  H3PO4+Aq  containing: 

10        20        30        40        50     %P2O5. 
1.1      1.23      1.39      -1.6      1.85 
(Dalton.) 


PHOSPHORIC  ACID 


673 


Sp.  gr.  of  H3PO4  +Aq. 

Sp.gr.  of  H3PO4  +  Aq  at  17  .  5°. 

Sp.gr. 

%  P=05 

Sp.  gr. 

%  P206      Sp.  gr. 

%  P205 

& 

Sp.  gr. 

% 
P206 

Sp.  gr. 

A 

Sp.  gr. 

1.508 
1.492 
1.476 
1.464 
1.453 
.442 
.434 
.426 
.418 
.401 
1.392 
1.384 
1.376 
1.369 
1.356 
1.347 
1.339 

49.60 
48.41 
47.10 
45.63 
45.38 
44.13 
43.95 
43.28 
42.61 
41.60 
40.86 
40.12 
39.66 
39.21 
38.00 
37.37 
36.74 

.328 
.315 
.302 
.293 
.285 
.276 
.268 
.257 
1.247 
1.236 
1.226 
1.211 
1.197 
1.185 
1.173 
1.162 
1.153 

36.15     1.144 
34.82     1.136 
33.49     1.124 
32.71     1.113 
31.94     1.109 
31.03     1.095 
30.13     1.081 
29.16     1.073 
28.24     1.066 
27.30     1.056 
26.36     1.047 
24.79     1.031 
23.23     1.022 
22.07     1.014 
20.91     1.006 
19.73 
18.81 

17.89 
16.95 
15.64 
14.33 
13.25 
12.18 
10.44 
9.53 
8.62 
7.39 
6.17 
4.15 
3.03 
1.91 
0.79 

1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 

1.007 
1.014 
1.021 
1.028 
1.036 
1.044 
1.053 
1.061 
1.070 
1.078 
1.086 
1.095 
1.103 
1.112 
1.120 
1.129 
1.139 
1.148 
1.158 
1.168 
1.178 
1.188 
1.198 

24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
34 
35 
36 
37 
38 
39 
40 
41 
42 
43 
44 
45 
46 

1.208 
1.219 
1.229 
1.240 
1.250 
1.261 
1.272 
1.282 
1.293 
1.304 
1.315 
1.326 
.338 
.350 
.362 
.374 
.386 
.398 
1.410 
1.423 
1.436 
1.448 
1.462 

47 
48 
49 
50 
51 
52 
53 
54 
55 
56 
57 
58 
59 
60 
61 
62 
63 
64 
65 
66 
67 
68 

1.476 
1,491 
1.505 
1.521 
1.536 
1.551 
1.566 
1.581 
1.597 
1.613 
1.629 
1.645 
1.661 
1.677 
1.693 
1.709 
1.725 
1.741 
1.758 
1.775 
1.792 
1.809 

(Watts,  C.  N.  12.  160.) 

Specific  gravity  of  H3PO4+Aq  containing: 
6             12             18      %H3P04, 
1.0333      1.0388      1.1065 

24             36             54      %H3PO4. 
1.1463      1.2338      1.3840 
(Schiff,  A.  113.  183.) 

Sp.  gr.  of  H3PO4+Aq  at  15°.    a=  sp.  gr.  if  % 
is  P2O5;  b=sp.  gr.  if  %  is  H3PO4. 

(Hager,  Adjumenta  varia,  Leipzig,  1876.) 

Table  for  correction  to  be  added  or  subtracted 
for  1°  change  in  temperature. 

% 

1 

2 
3 

4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 

a 

b 

% 

a 

b 

%  P2O6             Corr. 

%  P2O5              Corr. 

1:009 
1.017 
1.025 
1.032 
1.039 
1.047 
1.055 
1.063 
1.071 
1.080 
1.089 
1.098 
1.106 
1.115 
1.124 
1.133 
•1.142 
.151 
.161 
.171 
.182 
.192 
1.202 
1.212 
1.223 
1.233 
1.244 
1.254 
1.265 
1.277 

1.0054 
1.0109 
1.0164 
1.0220 
1.0276 
1.0333 
1.0390 
1.0449 
1.0508 
1.0567 
1.0627 
1.0688 
1.0749 
1.0811 
1.0874 
1.0937 
1.1001 
1.1065 
.1130 
.1196 
.1262 
.1329 
.1397 
1.1465 
1.1534 
1  .  1604 
1  .  1674 
1.1745 
1.1817 
1.1889 

31 
32 
33 
34 
35 
36 
37 
38 
39 
40 
41 
42 
43 
44 
45 
46 
47 
48 
49 
50 
51 
52 
53 
54 
55 
56 
57 
58 
59 
60 

1.288 
1.299 
1.310 
1.321 
1.333 
1.345 
1.357 
1.369 
1.381 
1.393 
1.407 
1.420 
1.432 
1.445 

1.1962 
1.2036 
1.2111 
1.2186 
1.2262 
1.2338 
1.2415 
1.2493 
1.2572 
1.2651 
1.2731 
1.2812 
1.2894 
1.2976 
1.3059 
1.3143 
1.3227 
1.3313 
1.3399 
1.3486 
1.3573 
1.3661 
1.3750 
1.3840 
1.3931 
1.4022 
1.4114 
1.4207 
1.4301 
1.4395 

10-14        0.00035 
15-25        0.0004 
26-35        0.00052 

36-45        0.00068 
46-55        0.00082 
56-68        0.001 

(Hager.) 
Sp.  gr.  of  H3PO4+Aq. 

G.-equivalents 
HsPO4  per  litre 

t° 

Sp.  gr.  t°/t° 

0.002572 
0.005142 
0.01025 
0.02042 
0.03056 
0.04065 
•j.,-507 
0.10046 
0.19951 
0.29716 
0.49057 
0.5070 
5.0700 

17.714 
17.706 
17.685 
17.683 
17.687 
17.704 
17.663 
17.696 
17.749 
17.701 
17.719 
17.58 
17.84 

1.001552 
1.0003051 
1.000595 
1.001158 
1.001708 
1.002252 
1.002790 
1.005412 
1.010560 
1.015584 
1.025469 
1.02627 
1.25162 

(Kohlrausch,  W.  Ann.  1894,  63.  29.) 

Miscible  with  cone.  HC2H3O2+Aq.     Sol. 
in  30  pts.  warm  creosote. 
1  cc.  of  a  sat.  solution  of  ether  in  H2O  dis- 
solves 0.0886  grams  H3PO4. 

(Schiff,  calculated  by  Gerlach,  Z.  anal.  8.  292.) 

674 


PHOSPHORIC  ACID 


1  cc.  of  a  sat.  solution  of  H2O  in  ether  dis- 
solves 0.000033  grams  H3PO4. 

Solutions  of  H3PO4  in  H2O  containing  less 
than  0.434  grams.acid  per  1  cc.  lose  an  insig- 
nificant amount  of  acid  to  ether  when  agi- 
tated therewith.  (Berthelot,  C.  R.  1896,  123. 
345.) 

The  composition  of  the  hydrates  formed  by 
H3PO4  at  different  dilutions  is  calculated  from 
determinations  of  the  lowering  of  the  fr.-pt. 
produced  by  H3PO4  and  of  the  conductivity 
and  sp.  gr.  of  H3PO4+Aq.  (Jones,  Am.  Ch. 
J.  1905,  34.  331.) 

10H3PO4+H2O.    Solubility  in  H2O. 
100  pts.  of  the  solution  contain  at: 

24.11°      24.38°      24.40° 

94.78        94.80       94.84  pts.  H3P04, 

24.81°      25.41°      25.85° 
94.95        95.26       95.54  pts.  H3PO4. 
(Smith  and  Menzies,  J.  Am.  Chem.  Soc.  1909, 
31.  1186.) 

2H3PO4+H2O.    Solubility  in  H2O. 
100  pts.  of  the  solution  contain  at: 
—16.3°    0.5°  14.95°  24.03°  27.0° 

76.7    78.7  81.7      85.7      87.7  pts.  H3P04, 


28.5C 
92.5 


29.15°      29.35°  (mpt.) 
90.5         91.6      pts.  H3P04, 

27.0°       25.41° 

93.4        94.1  pts.  H3PO4. 


Retroflex  part  of  curve. 
(Smith  and  Menzies,  J.  Am.  Chem.  Soc.  1909, 
31.  1186.) 

Pwrophosphoric  acid  (Diphosphoric  acid), 
H4P207. 

Very  sol.  in  H2O.  The  solution  may  be 
kept  without  change,  but  on  heating  it  is 
converted  into  H3PO4. 

The  acid  in  solution  gradually  changes  to 
H3PO4;  the  conversion  being  more  rapid  with 
more  concentrated  solutions.  (Montemartini 
and  Egidi,  Gazz.  ch.  it.  1902,  32.  (1)  381.) 

Phosphoric  acid,  H8P2O9  (?). 

Sol.  in  H2O.    (Joly,  C.  R.  100.  447.) 

Phosphates. 

The  phosphates  of  NH4,  K,  Na,  Li,  Cs,  and 
Rb  are  sol.  in  H2O,  with  the  exception  of 
certain  metaphosphates;  the  other  phosphates 
excepting  neutral  Tl  salts,  are  nearly  insol.  in 
H20,  excepting  when  an  excess  of  H3PO4  is 
present.  The  latter  are  all  sol.  in  HNO3+Aq. 

(a)  Metaphosphates. 

Monometaphosphates.  Only  alkali  mono- 
metaphosphates  are  known,  and  they  are  all 
insol.  in  H20. 


1  Dimetaphosphates.  Alkali  dimetaphos- 
phates  and  some  doublt  salts  containing  an 
alkali  as  one  of  the  bases  are  sol.  in  H2O,  the 
rest  are  si.  sol.  or  insol.  in  H2O. 

Tn'metaphosphates.  All  salts  are  sol.  in 
H20. 

Teirametaphosphates.  The  alkali  salts  are 
sol.  in  H2O,  the  others  are  insol. 

#e:rametaphosphates.  The  alkali  salts  are 
sol.,  the  others  insol.,  in  H2O,  but  are  mostly 
sol.  in  Na  hexametaphosphate+Aq. 

(6)  Orthophosphates.  K,  Na,  Li,  Cs,  and 
Rb  orthophosphates  are  sol.  in  H2O.  All  the 
others  are  insol.  in  H2O,  but  sol.  in  excess  of 
H3PO4,  and  HNO3+Aq;  less  easily  sol.  in 
HC2H3O2+Aq.  Pb,  Al,  and  Fe2  phosphates 
are  insol.  in  HC2H3O2+Aq.  SI.  sol.  in  NH4 
salts +Aq,  especially  NH4Cl+Aq,  from  which 
solution  they  are  pptd.  by  NH4OH+Aq. 
Orthophosphates  insol.  in  H2O  are  also  insol. 
in  an  excess  of  alkali  orthophosphates +Aq. 

All  orthophosphates  are  insol.,  or  very  si. 
sol.  in  alcohol. 

(c)  Pyrophosphates.  Alkali  pyrophos- 
phates  are  sol.  in  H2O;  the  others  are  insol. 
in  H2O,  but  are  mostly  sol.  in  an  excess  of  Na 
pyrophosphate + Aq . 

Aluminum  metophosphate,  A12(PO3)6. 

Insol.  in  H2O  and  cone,  acids.  (Maddrell, 
A.  61.  59.) 

Aluminum  or^ophosphate,  basic.  3A1203. 
P205  +  18H20. 

Min.  Evansite. 

4A12O3,  3P2O5  +  18H2O.  Ppt.  Insol.  in 
H2O.  (Rammelsberg.) 

2A1203,  P205. 

+3H2O.    Min.  Angelite. 

+5H2O.  Min.  Kalaite  (Turquoise).  Sol. 
in  HCl+Aq. 

+6H2O.  Decomp.  by  H2O.  (Hautefeuille, 
J.  pr.  (2)  37.  111.) 

Min.  Peganite.  More  or  less  sol.  in  HC1, 
and  HNO3+Aq. 

+8H2O.    Ppt.    (Munroe,  A.  159.  278.) 

Min.  Fischerite.  SI.  attacked  -by  HC1  or 
HNO3+Aq;  sol.  in  H2SO4+Aq. 

3A12O3,  2P2O5+8H2O,  or  12H2O.  Sol.  in 
acids,  even  after  ignition.  (Millot,  C.  R.  82. 
89.) 

+10H2O.  Min.  Caeruleolactite.  Sol.  in 
acids. 

+  12H2O.    Min.  Wavellite. 

Aluminum  or^ophosphate,  A12(PO4)2. 

Crystalline.  Not  attacked  by  cone.  HC1  or 
HNO3+Aq,  difficultly  by  hot  cone.  H2SO4. 
(de  Schulten,  C.  R.  98.  1583.) 

Ignited  A12(PO4)2  is  si.  decomp.  by  H2O,  so 
that  solubility  determinations  are  variable. 
For  an  extended  discussion,  see  original  paper. 
(Cameron  and  Hurst,  1904,  26.  898.) 


PHOSPHATE,  AMMONIUM 


675 


+4H2O.  Easily  sol.  in  mineral  acids,  inso 
in  acetic  and  other  organic  acids.  Easil 
sol.  in  KOH+Aq,  but  is  reprecipitated  fr 
NH4Cl+Aq.  Sol.  in  NH4OH+Aq.  Sol.  ii 
a  large  amount  of  alum+Aq  (Rose),  in 
aluminum  acetate  and  other  aluminum  salt 
+Aq  (Fleischer,  Z.  anal.  6.  28).  More  so 
than  ferric  phosphate  in  ammonium  oxalat< 
or  citrate +Aq.  (Millot.) 

Acid  I\H4  citrate +Aq  dissolves  3%  of  the 
P2O5;  neutral  NH4  citrate +Aq  dissolves  6.6 
of  the  P2O5;  ammoniacal  NH4   citrate + A. 
dissolves  completely  in  25  min.    (Erlenmeyer 
B.  14.  1869.) 

Sol.  in  NH4OH+Aq,  especially  in  presence 
of  alkali  phosphates,  (de  Koninck,  Z.  anal 
23.  90.) 

Not  pptd.  in  presence  of  alkali  tartrates  o: 
citrates,  sugar,  glycerine,  etc. 

Insol.  in  ethyl  acetate.  (Naumann,  B 
1910,  43.  314.) 

Min.  Variscite.  Very  quickly  sol.  in  warm 
cone.  HCl+Aq. 

+5H2O.    Min.  Zepharovitchite. 

+8H2O.    Min.  Gibbsite. 

Aluminum  or^/iophosphate.  acid,  2A12O3, 
3P205  +  16H20. 

Insol.  in  acids  after  being  ignited.  (Millot 
Bull.  Soc.  (2)  22.  244.) 

+4H2O,  and  6H2O.  Insol.  in  H2O  or  alco- 
hol. (Hautefeuille  and  Margottet,  J.  pr.  (2) 

A12O3',  2P2O5+8H2q.  Insol.  in  acids  or 
aqua  regia  after  being  ignited.  (Millot.) 

2A12O3,  5P2O5-{-14H2O.  Decomp.  by  cold 
H2O  into— 

4A12O3,  7P2O5+9H2O.  Decomp.  by  hot 
H2O.  (Erlenmeyer,  A.  194.  200.) 

A12O3,  3P2O5+3H2O=A12(H2PO4)6.  Deli- 
quescent; completely  sol.  in  a  little  cold 
H2O,  and  cone,  solution  can  be  boiled  without 
decomp.,  but  dil.  solution  (1  :  20)  separates 
A12(PO4)2  on  boiling,  which  redissolves  on 
cooling,  the  more  quickly  the  more  dilute  the 
original  solution.  (Erlenmeyer,  A.  194.  198.) 

Aluminum  pyrophosph&te,  A14(T2O7)3  + 
10H2O. 

Precipitate.  Sol.  in  mineral  acids,  and 
Na4P2O7+Aq;  insol.  in  acetic  acid.  Sol.  in 
KOH+Aq;  sol.  in  NH4OH+Aq,  but  when 
dissolved  in  HCl+Aq  is  reprecipitated  by 
NH4OH+Aq,  and  is  not  redissolved  in  an 
excess  thereof.  (Schwarzenberg,  A.  65.  147.) 

Sol.  in  alum+Aq.    (Rose,  Pogg.  76.  19.) 

Aluminum  pz/roraetaphosphate,  A12O3,  2P2O5. 
(Hautefeuille   and   Margottet,   C.   R.   96. 
849.) 

Aluminum  ammonium  dihydrogen  orthophos- 

phate,  NH4H2PO4,  A1PO4. 
Partially  decomp.  by  H2O.     Sol.  in  acids 
and  alkalies.    Nearly  insol.  in  50%  acetic  acid. 
(Cohen,  J.  Am.  Chem.  Soc.  1907,  29.  720.) 


Aluminum  calcium  phosphate,  A12O3,  3CaO, 
P205+3H20. 

Min.  Tavistockite. 

2A12O3,  6CaO,  3P2O5+3H2O.  Min.  Kirro- 
lite. 

Aluminum   calcium   phosphate   sulphate, 

3A12O3,  SO3,  Ca3(PO4)2+6H2O. 
Min.  Svanbergite.      Scarcely  attacked  by 
HCl+Aq,  and  only  si.  by  H2SO4+Aq. 

Aluminum    ferrous    magnesium    phosphate. 

(Mg,  Fe),Al2P2010+4H20. 
Min.  Childrenite.    Slowly  sol.  in  HCl+Aq.  • 
Min.  Eosphorite.     Sol.  in  HNO3  or  HC1  + 
Aq. 

(Mg,  Fe)Al2P2O9+H2O.  Min.  Lazulite. 
Only  si.  attacked  by  acids,  when  not  pre- 
viously ignited. 

Aluminum    lithium     phosphate,     A1->(PO4)2, 

4Li3PO4+30H2O. 
Precipitate.    (Berzelius.) 
Insol.  in  H2O;  easily  sol.  in  acids. 

Aluminum  magnesium  phosphate. 

Min.  Lazulite. 

See  Phosphate,  aluminum  ferrous  mag- 
nesium. 

Aluminum  potassium  phosphate,  A12O3,  K2O, 
2P205. 

Insol.  in  acids.  (Ouvrard,  A.  ch.  (6)  16. 
289.) 

2A12O3,  2K2O,  3P2O5.    (Ouvrard.) 

Aluminum    silver     raetophosphate,    2A12O8, 

Ag20,  4P205. 

(Hautefeuille  and  Margottet,  C.  R.  96.  849, 
1142.) 

Aluminum  sodium  pT/rophosphate, 
Al2Na2(P2O7)2. 

Insol.  in  H2O  and  acids.    (Wallroth.) 

Nearly  insol.  in  acids.  (Ouvrard.  A.  ch. 
6)  16.  338.) 

2A12O3,  3Na2O,  3P2O6.  Sol.  in  HNO3+Aq. 
Ouvrard.) 

A14(P2O7)3,  2Na4P2O7+30HoO. 

Very  difficultly  sol.  in  H2O.  (Pahl,  Bull. 
Soc,  (2)  22.  122.) 

iluminum   phosphate   lithium  fluoride, 

2A12(PO4)2,  3LiF. 

Min.  Amblygonite.  SI.  attacked  by  HC1+ 
^.q,  more  easily  by  H2SO4+Aq. 

Ammonium  wetophosphate,  NH4PO3. 
Insol.  in  H2O.    (Fleitmann,  Pogg.  78.  345.) 

Ammonium  dimetaphosphsde,  (NH4)2(PO8)2. 
Sol.  in  1.15  pts.  cold  or  hot  H2O.     (Fleit- 
mann,  Pogg.   78.   245.)      More  sol.   in  dil. 
Icohol  than  Na  or  K  salt. 


676 


PHOSPHATE,  AMMONIUM 


Sol.  in  0.9  pts.  H2O;  easily  sol.  in  acids 
pecially    by    boiling 
(Glatzel,  Dissert.  1880.) 


.  .          .  . 

especially    by    boiling    with    cone.    H2SO4. 
(Gla 


Ammonium  trimetaphosphate,  (NH4)3P3O9. 

Very  sol.  in  H2O.  (Lindbom,  Acta  Lund. 
1873.  15.) 

Ammonium  tetrametaphosphate, 
(NH4)4P4012. 

Sol.  in  H2O.  (Warschauer,  Z.  anorg.  1903, 
36.  177.) 

+4H2O.  Much  more  sol.  in  H2O  than  the 
K  or  Na  salt.  1  pt.  is  sol.  in  8  pts.  H2O. 
(Glatzel,  Dissert.  1880.) 

Ammonium  pentametaphosphate, 

(NH4)5P5015. 

Sol.  in  H2O.  (Tammann,  J.  pr.  1892,  (2) 
46.  455.) 

Ammonium  dekametaphosphate, 
(NH4)10P1003o. 

Very  si.  sol.  in  H2O;  100  g.  H2O  dissolved 
1.20-1.54  g.  in  2  months.  Easily  sol.  in  hot 
H2O  with  decomp.  (Tammann,  J.  pr.  1892, 
(2)  45.  448.) 

+  12H2O.    (Tammann,  J.  pr.  1892,  (2)  45. 


100  g.  H2O  dissolve  131  g.  at  15°;  sp.  gr. 
of  sat.  solution  =  1.343.  (Greenish  and 
Smith,  Pharm.  J.  1901,  66.  774.) 

Solubility  in  H3PO4+Aq  at  25°. 


In  1000  g.  of  the  solution,  mols. 

NH4 

P04 

6.42 

3.23 

6.46 

3.74 

6.56 

4.01 

6.78 

4.34 

7.26 

4.83 

7.16 

4.82 

(D'Ans  and  Schreiner,  Z.  phys.  Ch.  1910,  75. 
105.) 

Insol.  in  acetone.     (Eidmann,  C.  C.  1899. 
II,  1014;  Naumann,  B.  1904,  37.  4329.) 


Ammomum       ^hydrogen 
NH4H2PO4. 

Does  not  effloresce. 

Less  easily  sol.  in  H2O  than  (NH4)2HPO4. 
(Mitscherlich,  A.  ch.  19.  385.) 

Sol.  in  5  pts.  cold,  and  less  hot  H2O. 

Solubility  in  H8PO4+Aq  at  25°. 


100.; 

Ammomum    or^ophosphate,      (NH4)3PO4  + 
3H2O. 
Difficultly  sol.  in  H2O. 
Less  sol.  in  H2O  than  (NH4)2HPO4.    (Ber- 
zelius.) 
Insol.  in  alkalies  +Aq.    (Berzelius.) 
SI.    sol.    in   H2O.      Decomp.    in   the   air. 
(Schottlander,  Z.  anorg.  1894,  7.  344.) 

Solubility  in  H8PO4+Aq  at  25°. 

In  1000  g.  of  the  solution,  mols. 

NH4 

P04 

6.72 
5.62 
4.62 
2.72 
2.50 
2.58 
2.76 
3.06 
3.10 

4.54 
3.88 
3.36       . 
2.59 
2.54 
4.29 
6.21 
7.70 
7.86 

In  1000  g.  of  the  solution,  mols. 

(D'Ans  and  Schreiner,  Z.  phys.  Ch.  1910,  75. 
106.) 

Insol.  in  acetone.     (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 

Ammonium  o?-///ophosphate,  acid. 
Decomp.     into     NH4H2PO4     at     77-78°. 
(Parravano  and  Mieli,  Gazz.  ch.  it.  1908,  38, 
II.  536.) 

NH4 

PO4 

7.42 

5.02 
2.95 
3.04 
3.32 

4.78 

0.084 
0.20 
0.46 
1.02 
1.32 
2.32 

("TV  Ann  and  Sn.hrpinpr    7    nhvs    C!h    1Q10    75. 

105.) 

Insol.  in  acetone.     (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 
+5H2O.    (Sestini,  Gazz.  ch.  it.  9.  298.) 

Ammonium    hydrogen    or^ophosphate, 
(NH4)2HP04. 

Easily  sol.  in  H2O.     Effloresces  to  form 
NH4H2PO4.    (Schiff,  A.  112.  88.) 

Sol.  in  4  pts.  cold,  and  less  hot  H2O.    Solu- 
tion loses  NH3  by  boiling.    Insol.  in  alcohol. 


Ammonium  p?/r0phosphate,  (NH4)4P2O7. 

Easily  sol.  in  H2O.  Alcohol  precipitates  it 
from  the  aqueous  solution.  (Schwarzenberg, 
A.  65.  141.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 

Ammonium  hydrogen  p?/rophosphate 

(NH4)2H2P207. 

Very  sol.  in  H2O.  Insol.  in  alcohol. 
(Schwarzenberg,  A.  65.  141.) 


PHOSPHATE,  AMMONIUM  MAGNESIUM 


677 


Ammonium  barium  trimetaphospha.te, 

(NH4)BaP3O9+H2O. 
Easily  sol.  in  H2O.    (Lindbom.) 

Ammonium  cadmium  cfo'raetaphosphate, 
(NH4)2O,  CdO,  2P2O5+3H2O  = 
(NH4)2Cd(P2OG)2. 
Efflorescent.     (Fleitmann,  Pogg.  78.  347.) 

Ammonium  cadmium  orZ/iophosphate, 

NH4CdPO4+li/4H2O. 
Easily    sol.    in    NH4OH+Aq    and    acids. 
(Drewson,  Gm.  K.  Handb.  6te  Aufi.  III.  74.) 

Ammonium  calcium  dimetaphosphaie, 

(NH4)2Ca(P2O6)2-f2H2O. 
Very  si.  sol.  in  H2O.     Not  decomp.  by 
acids.    (Fleitmann,  Pogg.  78.  344.) 

Ammonium  calcium  phosphate,  !SH4CaPO4  + 


Ppt.  (Herzfeld  and  Feuerlein,  Z.  anal.  20. 
191.) 

-j-7H2O.  Not  completely  decomp.  by  cold 
H2O  in  y\  hour;  rapidly  by  hot  H2O.  (Lasne, 
Bull.  Soc.  1902,  (3)  17.  131.) 

Ammonium  chromium  or^ophosphate,  basic, 

5(NH4)H2PO4,  2CrPO4,  4Cr(OH)3. 
(Cohen,  J.  Am.  Chem.  Soc.  1907,  29.  1196.) 
(NH4)2HPO4,        2CrPO4+3H2O.          Ppt. 

(Cohen.) 

Ammonium  chromic  pyro  phosphate, 

NH4fCrP207)+6H20. 
SI.  sol.  in  cold  H2O.     Decomp.  by  boiling 
H2O.    (Rosenheim,  B.  1915,  48.  586.) 

Ammonium  cobaltous  wefaphosphate. 

Extremely  sol.  in  H2O  and  in  NH4OH+Aq. 
(Persoz,  J.  pr.  3.  215.) 

Ammonium  cobaltous  or^Aophosphate, 

NH4CoPO4+H,O. 
Not  decomp.  by  boiling  H2O.    (Debray,  J. 

Pharm.  (3)  46.  121.) 

+  12H2O.    Ppt.    (Chancel,  1862.) 
Co(NH4)2H2(PO4)2+4H2O.    Insol.  in  H2O. 

(Debray.) 


Ammonium  copper  cfo' 

(NH4)2P206,  CuP2Oc+2H2O. 

Very  si.  sol.  in  H2O;  insol.  in  alcohol. 
(Fleitmann,  Pogg.  78.  345.) 

+4H2O.  Efflorescent.  Very  si.  sol.  in 
H2O;  insol.  in  alcohol.  (F.) 

Sol.  in  50  pts.  H2O.  Slowly  attacked  by 
acids.  Only  boiling  H2SO4  attacks  easily. 
(Glatzel,  Dissert.  1880.) 

Ammonium    glucinum    orZ/iophosphate, 

NH4G1PO4. 

Insol.  in  cold,  si.  sol.  in  hot  H2O.  (Rossler, 
Z.  anal.  17.  148.) 


Ammonium  glucinum  sodium  orZ/iophosphate, 

(NH4)2GlNa2(PO4)2+7H2O. 
(Scheffer,  A.  109.  146.) 

Ammonium  iron  (ferrous)  ort/iophosphate, 
NH4FePO4+H2O. 

Insol.  even  in  boiling  H2O.  When  still 
moist,  easily  sol.  in  dil.  acids,  but  sparingly 
and  slowly  sol.  after  drying,  even  in  cone, 
acids.  Decomp.  by  NH4OH,  KOH,  and 
NaOH+Aq.  Insol.  in  alcohol.  (Otto,  J.  pr. 
2.  409.) 

(NH4)2FeH2(PO4)2+4H2O.    (Debray.) 

Ammonium  iron  (ferric)  hydrogen  orthophos- 
phate,    basic,    2(NH4)2HPO4,    3FePO4, 
3Fe(OH)3. 
Ppt.     Insol.  in  95%  alcohol.     (Cohen,  J. 

Am.  Chem.  Soc.  1907,  29.  719.) 

Ammonium  iron  (ferric)  hydrogen  orthophos- 
phate,  NH4H2Fe(PO4)2. 

Ppt.  Same  properties  as  Na  salt.  (Wein- 
land,  Z.  anorg.  1913,  84.  356.) 

Partially  hydrolyzed  by  H2O.  Readily  sol. 
in  HC1,  HNO3,  H2S04  and  H3PO4.  Partially 
hydrolyzed  by  cold  NH4OH+Aq.  Sol.  in 
excess  of  hot  NH4OH+Aq.  Completely 
hydrolyzed  by  caustic  alkalies.  Practically 
insol.  in  50%  acetic  acid.  (Cohen,  J.  Am. 
Chem.  Soc.  1907,  29.  718.) 

Ammonium  lead  cfo'raeZaphosphate, 

(NH4)2Pb(P206)2. 

Very  difficultly  sol.  in  H2O  and  acids. 
(Fleitmann,  Pogg.  78.  343.) 

Ammonium     lithium    metophosphate,    Li2O, 

2(NH4)2O,   3P2O5+8H2O. 
Not   appreciably  sol.    in    cold  H2O    but 
rapidly  and  abundantly  sol.  in  H2O  at  70°. 
(Tammann,  J.  pr.  1892,  (2)  45.  442.  ) 

Ammonium  lithium  phosphate,  (NH4)2LiPO4. 
SI.  sol.  in  H2O.    (Berzelius.) 

Ammonium  magnesium  wetaphosphate, 
(NH4)20,  2MgO,  2P205+9H20  (?). 

Sol.  with  difficulty  in  H2O  or  acids  when 
heated.  Easily  sol.  in  H2O  before  heating. 
(Wach,  Schw.  J.  59.  29.) 

Precipitated  from  aqueous  solution  by 
alcohol. 

Ammonium     magnesium     cfo'w-etaphosphate, 

(NH4)2Mg(P206)2+6H20. 
Efflorescent.    (Fleitmann,  Pogg.  78.  346.) 

Ammonium  magnesium  phosphate, 
NH4MgPO4,  and  +6H2O. 

1  1.  H2O.  dissolves  66  mg.  anhj^drous 
NH4MgPO4  at  15°.  (Fresenius,  A.  55.  109.) 

1  1.  H2O  dissolves  74.1  mg.  anhydrous 
NH4MgPO4  at  20.5-22.5°.  (Ebermayer.) 


678 


PHOSPHATE,  AMMONIUM  MAGNESIUM  HYDROGEN 


1  1.  H2O  dissolves  106  mg.  anhydrous 
NH4MgPO4.  (Liebig.) 

Insol.  in  H2O,  but  when  boiled  with  H2O  it 
loses  NH3  and  H2O.  (Struve,  Z.  anal.  1898, 
37.  485.) 

Solubility  of  NH4MgPO4+6H2O  in  H2O  at  t°. 


t° 

G.  salt  in  100  g.  H2O 

0 
20 
40 
50 
60 
70 
80 

0.0231 
0.0516 
0.0359 
0.0303 
0.0401 
0.0163 
0.0195 

(Wenger,  Dissert.  Geneva,  1911.) 

Aqueous  solution  is  precipitated  by 
NH4OH,  but  not  by  Na2HPO4+Aq.  (Fre- 
senius.) 

Sol.  in  44,600  pts.  H2O  containing  am- 
monia. More  sol.  in  H2O  containing  NH4C1, 
and  is  sol.  in  7548  pts.  of  a  solution  containing 
1  pt.  NH4C1  to  5  pts.  H2O  and  ammonia,  and 
in  15,627  pts.  of  a  solution  containing  1  pt.  of 
NH4C1  to  7  pts.  H2O  and  ammonia.  (Fre- 
senius.) 

According  to  Kremers  (J.  pr.  65.  190),  a 
solution  of  3  pts.  H2O  to  1  pt.  NH4OH+Aq 
of  0.96  sp.  gr.  is  best  suited  for  washing  the 
precipitated  NH4MgPO4. 

According  to  Ebermayer  (J.  pr.  60.  41), 
1  pt.  anhydrous  salt  is  sol.  in  13,497  pts. 
H2O  at  23°;  in  31,098  pts.  NH4OH+Aq  (4 
pts.  H2O:  1  pt.  NH4OH+Aq  of  0.961  sp.  gr.) 
at  21.25°;  in  36,764  pts.  NH4OH+Aq  (3  pts. 
H2O:  1  pt.  NH4OH+Aq)  at  20.6°;  in  43,089 
pts.  NH4OH+Aq  (1  pt,  H2O:  1  pt.  NH4OH  + 
Aq)  at  22.5°;  in  45,206  pts.  NH4OH+Aq 
(1  pt.  H2O:  2  pts.  NH4OH+Aq)  at  22.5°;  in 
52,412  pts.  NH4OH+Aq  (1  pt.  H2O:  3  pts. 
NH4OH+Aq)  at  22.5°;  in  60,883  pts.  pure 
NH4OH+Aq  (sp.  gr.  0.961)  at  22.5°. 

Almost  absolutely  insol.  in  H2O  containing 
K  vol.  NH4OH+Aq  (sp.  gr.  0.96)  and  NH4C1, 
i.e.,  much  more  insol.  than  given  by  Fresenius. 
(Kubel,  Z.  anal.  8.  125.) 

According  to  Kissel  (Z.  anal.  8.  173),  1  1. 
NH4OH+Aq  (3  pts.  H2O:  1  pt.  NH4OH+Aq 
of  0.96  sp.  gr.)  dissolves  4.98  mg.  in  24  hours, 
while  13.9  mg.  are  dissolved  if  18  g.  NH4C1  to 
a  litre  of  H2O  are  also  present. 

(NH4)2SO4+Aq  containing  2.2  g.  per  litre 
dissolves  71.7  mg.;  3.0  g.,  113  mg.;  10  g., 
147  mg.;  NaCl+Aq  containing  2  g.  NaCl  per 
1.  dissolves  123.4  mg.;  NaNO3-j-Aq  containing 
3  g.  NaNO3  per  1.  dissolves  93.1  mg.  (Liebig, 
A.  106.  196.) 

Completely  insol.  in  water  containing  am- 
monium phosphate  or  ammonium  sodium 
phosphate.  (Berzelius.) 

800  com.  H2O,  sat.  with  CO2,  dissolve  1.425 
g.  (Liebig.) 

Easily  sol.  in  H2SO3+Aq,  acetic  and  other 


acids,  also  in  boiling  solution  of  ammonium 
citrate.  (Millot,  Bull.  Soc.  (2)  18.  20.) 

When  in  presence  of  Fe  or  Al  salts  it  is  sol. 
to  a  considerable  extent  in  H2C4H406+Aq. 

6  g.  NH4C1  in  100  ccm.  H2O  containing  10 
ccm.  6.34%  NH4OH+Aq  dissolve  pptd.  salt 
=  0.0029  g.  Mg2P2O7.  1  g.  (NH4)2C2O4  in 
100  ccm.  H2O,  and  NH4OH+Aq  dissolve  = 
0.0061  g.  Mg2P2O7.  2  g.  citric  acid  in  excess 
of  NH4OH+Aq  dissolve  =  0.0147  g.  Mg2P2O7. 
Solubility  prevented  by  excess  of  magnesia 
mixture.  (Lindo,  C.  N.  48.  217.) 

Solubility  of  NH4MgPO4+6H2O  in  salts+Aq 
at  t°. 

(G.  salt  dissolved  in  100  g.  solvent.) 


t° 

5%  NH4N03 
+Aq. 

5% 
NH4Cl+Aq. 

1  pt.  NH4OH 
(D  =0.96) 
+4  pts.  EhO 

0 

0.1100 

0.0597 

0.0087 

20 

0.0463 

0.1055 

0.0098 

30 

0.0546 

0.1133 

40 

0.0645 

0.0713 

0.6135 

50 

0.0723 

0.0931 

0.0153 

60 

0.0846 

0.1728 

0.0174 

70 

0.0834 

0.1239 

0.0178 

80 

0.1009 

0.1913 

0.0145 

t° 

4%  NH4OH+Aq  and 
5%NH4Cl+Aq. 

4%  NH4OH  +Aq  and 
10%  NH4Cl+Aq. 

20 
60 

0.0165 
0.0274 

0.0541 
0.0731 

(Wenger,  Dissert.  Geneva,  1911.) 

About  3  times  as  sol.  in  €a(C2H302)2+Aq 
as  in  NaC2H3O2+Aq,  but  solubility  is  pre- 
vented by  excess  of  MgCl2.  (Ville,  Bull.  Soc. 
(2)  18.  316. 

SI.  sol.  in  ammonium  citrate +Aq  contain- 
ing 400  g.  ammonium  citrate  in  a  litre. 
Solubility  =  0.457%  at  ord.  temp,  and  0.58% 
at  50°.  (Bolis,  Ch.  Z.  1903,  27.  1151.) 

Min.  Struvite. 

+HoO.  Insol.  in  H2O  or  citric  acid+Aq. 
(Millot  and  Maquenne,  Bull.  Soc.  (2)  23.  238.) 

Ammonium  magnesium  hydrogen  orthophos- 

phate,  (NH4)2MgH2(P04)2+3H20  (?). 
(Graham.) 

Ammonium  magnesium  phosphate, 

5MgO,  (NH4)2O,  2P2O5+24H2O. 
(Gawalovsky,  C.  C,  1885.  721.) 

Ammonium   magnesium    sodium   pyrophos- 

phate,  fNH4)3Mg6Na(P207)4. 
Insol    in  H2O  and  not  decomp.  thereby. 
(Berthelot  and  Andre",  A.  ch.  1897,  (7)  11. 
186.) 


PHOSPHATE,  AMMONIUM  SODIUM 


679 


Ammonium  manganous  c^wetaphosphate, 
(NH4)2Mn(PO8)4+4H2O. 

Relatively  easily  attacked  by  acids.  (Glat- 
zel,  Dissert!  1880.) 

+6H20. 

Efflorescent.    (Fleitmann,  Pogg.  78.  346.) 

Ammonium  manganous  or^ophosphate, 
NH4MnPO4+H2O. 

Sol.  in  32,092  pts.  cold,  and  20,122  pts. 
boiling  H2O,  and  in  17,755  pts.  NH4Cl+Aq 
(1.4%  NH4C1).  (Fresenius.) 

+7H2O.  Insol.  in  H2O  below  70°;  at  70° 
100  g.  H2O  dissolve  0.0052  g.  salt;  at  80°, 
0.0067.  (Wenger,  Dissert.  Geneva,  1911.) 

Easily  sol.  in  dil.  acids.  Decomp.  by 
KOH+Aq,  but  not  by  NH4OH+Aq  or 
K2CO3+Aq.  Insol.  in  NH4OH  or  NH4  salts 
+Aq.  (Gibbs.) 

Solubility  in  salts +Aq  at  t°. 
(G.  in  100  g.  solvent.) 


t° 

5% 
NH4NO 

+Aq. 

5% 
NH4Cl+Aq. 

1  pt.  NH4OH 
D  =0.96 
+4  pts.  H2O. 

0 

0.0206 

0.0020 

0.0116 

20 

0.0200 

0.0255 

0.0122 

30 

0.0226 

0.0345 

40 

0.0209 

0.0386 

0.0118 

50 

0.0226 

0.0355 

0.0132 

60 

0.0270 

0.0384 

0.0193 

70 

0.0281 

0.0414 

0.0191 

80 

0.0326 

0.0451 

0.0197 

(Wenger,  L  c.) 

Insol.  in  alcohol. 

Insol.  in  acetone.  (Naumann.  B.  1904,  37. 
4329.) 

Ammonium  manganic  pyrophosphate. 

NH4MnP2O7+3H2O. 

Decomp.  bv  cold  H2O  with  separation  of 
Mn2O3.  (Rosenheim,  B.  1915,  48.  584.) 

Ammonium   manganous    sodium   pyrophos- 
phate,  NH4NaMnP2O7+3H2O. 

Insol.  in  H2O  or  alcohol.  Easily  sol.  in  very 
dil.  acids.  (Otto,  J.  pr.  2.  418.) 

formula   is    Na4(NH4)4Mn2(P2O7)3  + 
12H2O,  according  to  Berzelius. 

Ammonium  mercuric  metaphosphate. 

Sol.  in  H2O,  or  at  least  in  NH4OH+Aq. 
(Persoz,  J.  pr.  3.  216.) 

Ammonium  nickel  metaphosphate. 

Insol.  in  H2O.  Sol.  in  NH4OH+Aq,  from 
which  it  is  repptd.  on  evaporation  of  the  NH3. 
(Persoz,  J.  pr.  3.  215.) 

Ammonium  nickel  dimetaphosphate, 

(NH4)2NiP4012+4H20. 
Sol.  in  12.5  pts.  H2O.     (Glatzel,  Dissert. 
1880.) 


Ammonium    nickel   or^ophosphate, 

•   NH4NiPO4+2H2O. 

Ppt.    (Debray,  C.  R.  69.  40.) 

+6H2O.    Decomp.  by  boiling  H2O.    (De- 
bray.) 

Ammonium  potassium  dimetaphosphate, 
(NH4)ioK<(P,0,)7. 

More   sol.    in   H2O    than    following    salt. 
(Fleitmann,  Pogg.  78.  341.) 

NH4K3P4O12+2H2O.      Difficultly    sol.    in 
H2O.    (Fleitmann.) 

Ammonium  potassium  pz/rophosphate, 


Deliquescent.  Sol.  in  H2O.  Decomp.  on 
boiling.  (Schwarzenberg.) 

Ammonium  sodium  dimeiaphosphatej 

NH4NaP2O6+H2O. 

More  sol.  in  H2O  than  Na2P2O6,  but  less 
than  (NH4)2PaOe.  Less  sol.  in  alcohol  than 
in  H2O.  (Fleitmann,  Pogg.  78.  340.) 

Ammonium  sodium  ori/iophosphate, 
(NH4)2NaPO4+4H2O. 

Decomp.  by  H2O.  Cryst.  from  NH4OH  + 
Aq  of  0.96  sp.  gr.  From  H2O  solution, 
NaNH4HPO4+4H,O  separates  out.  (Uels- 
mann,  Arch.  Pharm.  (2)  99.  138.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

+5H2O. 

NH4Na2PO4+12H2O.  (Herzfeld,  Z.  anal. 
20.  191.) 

(NH4)5Na(PO4)2+6H2O.  Sol.  in  H2O  with 
decomp.  Cryst.  from  hot  cone.  NH4OH+Aq. 
(Uelsmann,  Arch.  Pharm.  (2)  99.  138.) 

Ammonium  sodium  hydrogen  phosphate  (Mi- 
crocosmic  salt),  NH4NaHPO4+4H2O. 

Efflorescent.  Easily  sol.  in  H2O.  Sol.  in  6 
pts.  cold,  and  1  pt.  boiling  H2O.  Insol.  in 
alcohol. 

Aqueous'  solution  gives  off  NH3,  especially 
if  hot. 

Insol.  in  acetone.  (Eidmami,  C.  C.  1899, 
II.  1014.) 

Min.  Stercorite. 

+5H2O.    (Uelsmann.) 

The  composition  of  the  hydrates  formed  by 
this  salt  at  different  dilutions  is  calculated 
from  determinations  of  the  lowering  of  the 
fr.-pt.  produced  by  the  salt  and  of  the  con- 
ductivity and  sp.  gr.  of  its  aqueous  solutions. 
(Jones,  Am.  Ch.  J.  1905,  34.  319.) 

(NH4)3Na3H6(PO4)4+3H2O.  Decomp.  by 
H20.  (Filjiol  and  Sendereng,  C.  R.  93.  388.) 

Ammonium  sodium  p^/rophosphate, 
(NH4)2Na2P2O7+5H2O. 

Easily  sol.  in  H2O.  Aqueous  solution  de- 
comp. fcy  boiling.  (Schwarzenberg,  A.  65. 
142.) 

+6H2O.    (Rammelsberg.) 


680 


PHOSPHATE,  AMMONIUM  SODIUM  GLUCINUM 


Ammonium  sodium  glucinum  or/Aophosphate, 

(NH4)2Na2Gl(PO4)2+7H2O. 
Precipitate.    (Scheffer.) 

Ammonium  thallous  orZAophosphate, 

(NH4)3P04,  (NH4)2T1P04,  or  H2NH4P04, 
HT12PO4. 
Sol.  in  H2O.    (Lamy;  Rammelsberg.) 

Ammonium  uranyl  phosphate, 
NH4(U02)P04+o;H20. 

Insol.  in  H2O  and  HC2H3O2+Aq.  Sol.  in 
mineral  acids,  from  which  it  is  precipitated 
by  NH4C2H3O2+Aq,  in  which  it  is  insol'. 
(Knop.) 

+3H2O.  Insol.  in  H2O  and  acetic  acid. 
Sol.  in  all  mineral  acids,  oxalic  acid  and 
M2CO3+Aq.  (Lienau,  Dissert.  1898.) 

Ammonium  vanadium  phosphate. 
See  Phosphovanadate,  ammonium. 

Ammonium  zinc  e&wetaphosphate, 

(NH4)2Zn(P206)2+6H20. 
Efflorescent.    (Fleitmann,  Pogg.  78.  347.) 
+4H2O.    Sol.  in  70  pts.  H2O.    Decomp.  by 
H2SO4.    (Glatzel,  Dissert.  1880.) 

Ammonium  zinc  or^ophosphate,  basic, 
3NH3,  2ZnO,  P2O5+8H2O. 

(Rother,  A.  1867,  143.  356.) 

4(NH4)  A  6ZnO,  3P2O5+4H2O.  (Schweik- 
ert,  A.  1868,  146.  57.) 

Ammonium  zinc  or/ftophosphate,  NH4ZnPO4 

+H20. 

Insol.  in  H2O.  Sol.  in  acids,  and  caustic 
alkalies.  (Bette,  A.  15.  129.) 

Ammonium  zinc  hydrogen  phosphate, 
NH4H2PO4,  ZnHPO4+H2O. 

Insol.  in  H2O.    (Debray.) 

4(NH4)2O,  6ZnO,  3P2O5.  (Schweikert,  A. 
146.  57.) 

3(NH4)2O,  4ZnO,  2P2O5  +  13H2O.  (Rother, 
A.  143.  356.) 

Ammonium  phosphate  selenate. 
See  Selenophosphate,  ammonium. 

Barium  /riphosphate,  5BaO,  3P2O6. 

Insol.  in  H2O;  insol.  in  acids  after  heating 
to  a  high  temp.  (Schwarz,  Z.  anorg.  1895,  9. 
264.) 

Barium  raetophosphate,  Ba(PO3)2. 

Insol.  in  H>O  or  dil.  acids.  (Maddrell,  A. 
61.  61.) 

Not  decomp.  by  boiling  with  acids  or  alkali 
carbonates +Aq.  (Fleitmann,  Pogg.  78.  352.) 

Barium  cfo'wetophosphate,  BaP2O6+2H2O. 

More  difficultly  sol.  in  H2O  than  Ba3(P3O9)2. 
Slightly  attacked  by  boiling  cone.  HCl+Aq 
or  HNO3+Aq.  Easily  decomp.  by  H2SO4. 
(Fleitmann,  Pogg.  78.  254.) 


Barium  Zrmetaphosphate,  Ba3(P3O9)2+2H2O. 

Somewhat  sol.  in  H2O.  (Fleitmann,  A.  65. 
313.) 

+6H2O.  Easily  sol.  in  HCl+Aq.  (Lind- 
bom.) 

1  1.  H2O  dissolves  2.589  g.  at  ord.  temp. 
(Wiesler,  Z.  anorg.  1901,  28.  "198.) 

Barium  hexametaphosph&te,  Ba3P6O,8  (?). 

Sol.  in  H2O  only  after  boiling  several  hours. 

Nearly  insol.  in  H2O.  (Liidert,  Z.  anorg. 
6.  15.) 

Insol.  in  NH4Cl+Aq.    (Wackenroder.) 

Sol.  in  Na6P6O18+Aq.  Sol.  in  HNO,+Aq. 
After  ignition  it  is  nearly  insol.  in  HNO3+Aq. 

Barium  ort/iophosphate,  Ba3(PO4)2. 

Precipitate.  Very  si.  sol.  or  insol.  in  H2O. 
(Graham,  Pogg.  32.  49.) 

Sol.  in  HCl+Aq.     Decomp.  by  SO2+Aq. 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Barium  hydrogen  phosphate,  BaHPO4. 

Sol.  in  10,000  pts.  H2O.  (Malaguti,  A.  ch. 
(3)  61.  346.) 

Sol.  in  20,570  pts.  H2O  at  20°.  (Bischof, 
1833.) 

Not  completely  soluble  in  water  containing 
CO2,  but  BaCl2  causes  no  ppt.  in  Na2HPO4+ 
Aq  containing  7.16  g.  or  less  Na2HPO4  in  a 
litre  after  it  has  been  saturated  with  CO2. 
(Setschenow,  C.  C.  1876.  97.) 

Easily  sol.  in  H3PO4+Aq,  and  dil.  HC1+ 
Aq.  HNO3 + Aq  of  1 .275  sp.  gr.  if  not  diluted 
has  scarcely  any  solvent  action,  but  more  dis- 
solves on  dilution  until  a  maximum  is  reached, 
when  10  vols.  of  H2O  have  been  added. 
(Bischof,  Schw.  J.  67.  39.) 

Sol.  in  367-403  pts.  acetic  acid  (1.032  sp. 
gr.)  at  22.5°.  (Bischof,  I.  c.) 

Easily  sol.  in  H2O  containing  NH4C1, 
NH4NO3,  or  NH4  succinate,  from  which  solu- 
tions it  is  completely  pptd.  by  NH4OH+Aq. 
(Rose.) 

Insol.  in  Na2HPO4  or  BaCl2+Aq.  (Rose, 
Pogg.  76.  23.) 

More  sol.  in  BaCl2  or  NaCl+Aq  than  in 
H2O,  1  pt.  BaHPO4  being  sol.  in  4362  pts. 
H2O  containing  1.2%  NaCl  and  0.8%  BaCl2. 
(Ludwig,  Arch.  Pharm.  (2)  56.  265.) 

Sol.  in  Na  citrate +Aq.    (Spiller.) 

Barium  tefrahydrogen  phosphate, 

BaH4(PO4)2. 

Sol.  in  H2O.    (Mitscherlich,  1821.) 
Decomp.    by    much    H2O    into    BaHPO4. 

Sol.  in  phosphoric,  and  certain  other  acids. 

(Berzelius,  A.  ch.  2.  153.) 

Barium  pi/rophosphate,  Ba2P2O7+zH2O. 

Somewhat  sol.  in  H2O,  in  much  H4P2O7  + 
Aq,  also  in  HCl+Aq  or  HNO3+Aq.  Insol. 
in  HC2H3O2  +  Aq  or  Na4P2O7  +  Aq.  (Schwar- 
zenberg.) 

Insol.  in  NH4Cl+Aq.     (Wackenroder.) 


PHOSPHATE,  BORON 


681 


Barium  hydrogen  pyrophosphate, 

Ba2P2O7+3H2O. 
Ppt.    (Knorre  and  Oppelt,  B.  21.  773.) 

Barium  te£raphosphate,  Ba3P4Oi3. 

Insol.  in  H2O  or  acids  when  strongly  heated. 
(Fleitmann  and  Henneberg,  A.  65.  331.) 

Barium  manganic  pyrophosphate, 

Ba(MnP2O7)2+5H2O. 

Almost   insol.    in    H2O.      (Rosenheim,    B. 
1915,  48.  585.) 


Barium  potassium  fn'mefaphosphate, 
BaKP3O9+H2O. 

Much  less  sol.  in  H2O  than  NH4BaP3O9  or 
NaBaP3O9.  (Lindbom.) 

Sol.  in  HCl+Aq  after  ignition. 

Barium  potassium  or^ophosphate,  BaKPO4. 

Insol.  in  H2O.  (Ouvrard,  A.  ch.  (6)  16. 
297.) 

+  10H2O.    (de  Schulten,  C.  R.  96.  706.) 

Barium  sodium  diwefaphosphate, 

BaNa.(P2O6)2+4H2O. 
(Glatzel,  Dissert.  1880.) 

Barium  sodium  £n'we£aphosphate,  BaNaP3O9 
+4H20. 

More  easily  sol.  in  1I2O  than  Ba3(P3O9)2. 
Sol.  in  acids,  unless  ignited.  (Fleitmann  and 
Henneberg,  A.  65.  314.) 

Efflorescent.  Sol.  in  HCl+Aq  after  igni- 
tion only  by  long  boiling.  When  fused  it  is 
easily  sol.  in  HCl+Aq.  (Lindbom,  Acta 
Lund.  1873.  21.) 

Barium  sodium  orZ/iophosphate,  BaNaPO4  + 
10H2O. 

(de  Schulten,  C.  R.  96.  706.) 

Not  attacked  by  cold,  but  decomp.  by  hot 
H2O.  (Villiers,  C.  R.  104.  1103.) 

SI.  sol.  in  H2O.  (Quartaroli,  C.  A.  1911. 
2375.) 

Barium  sodium  pi/rophosphate, 
Ba4Na4(P2O7)s. 

Sol.  in  hot  HC1  and  HNO3.  (Tammann, 
J.  pr.  1892,  (2)  45.  469.) 

6Ba2P2O7,  Na4P2O7+6H2O.  Completely 
insol.  in  Na4P2O7+Aq,  but  not  insol.  in  H2O 
or  NH4OH+Aq.  Easily  sol.  in  HNO8  or  HC1 
+Aq.  Insol.  in  alcohol.  (Baer,  Pogg.  75. 
164.) 

Barium  uranous  metaphosphate,  UO2,  BaO, 

P205. 
(Colani,  A.  ch.  1907,  (8)  12.  142.) 


Barium  uranyl  ori/iophosphate, 

Ba(UO2)2(PO4)2+8H2O. 
Min.  Uranocirrite. 

Barium  phosphate  chloride,  3Ba3(PO4)2, 
BaCl2. 

Min.  Barytapatite.  (Deville  and  Caron,  A. 
ch.  (3)  67.  451.) 

4BaH4(PO4)2,  BaCl2.  (Erlenmeyer,  J.  B. 
1857.  145.) 

ISBaO,  6P2O5,  BaCl2+6H2O  (?).  Sol.  in 
18,000  pts.  cold  H2O.  Much  more  sol.  in  H2O 
containing  BaCl2,  NH4C1,  and  NH4OH. 
(Ludwig,  Arch.  Pharm.  (2)  56.  271.) 

Bismuth      ortftophosphate,     basic,     2BiPO4, 

3Bi2O8. 

Insol.  in  H2O.  Sol.  in  HCl+Aq.  (Cavazzi, 
Gazz.  ch.  it.  14.  289.) 

Bismuth  or/ftophosphate,  BiPO4. 

Insol.  in  H2O  or  HNO3+Aq.  SI.  sol.  in 
NH4  salts+Aq.  (Chancel,  C.  R.  50.  416.) 

Not  decomp.  by  H2O.  Other  phosphates 
of  Bi  are  decomp*.  by  H2O.  (Montmartini, 
C.  C.  1900,  II.  1256.) 

Not  hydrolyzed  by  hot  H2O;  si.  sol.  in  BiCls 
+Aq;  decomp.  by  boiling  alkali.  (Caven, 
J.  Soc.  Chem.  Ind.  1897,  16.  30.) 

More  sol.  in  HCl+Aq  than  in  HNO3+Aq. 
(Rose.) 

Sol.  in  UO2(NO3)2+Aq.  (M'Curdy,  Am.  J. 
Sci.  (2)  31.  282.) 

Insol.  in  MNO3+Aq. 

Insol.  in  Bi  salts+Aq.  (Rose,  Pogg.  76. 
26.) 

Sol.  in  NH4Cl+Aq,  but  insol.  in  NH4NO3  + 
Aq.  (Brett,  1837.) 

+  1^H2O.    (Kiihn.) 

+3H2O.  Ppt.  Decomp.  by  H2S  or  KOH 
+Aq.  (Vanino,  J.  pr.  1906,  (2)  74.  151.) 

Bismuth  p^/rophosphate,  basic,  2Bi«Os,  P2O5. 
Insol.  in  H2O  and  HC2H3O2+Aq;  sol.  in 
hot  HC1  and  HNO.+Aq.  Insol.  in  Na4P2O7 
+Aq,  and  NH4  citrate +Aq.  (Passerini, 
Cim.  9.  84.) 

Bismuth  pi/rophosphate,  Bi4(P2O7)3/ 

Insol.  in  H-O  or  HNO3+Aq.     (Chancel, 

C.  R.  50.  416.) 

Decomp.  by  H2O.    (Wallroth,  Bull.  Soc.  (2) 

39.  316.) 

Sol.  in  Na4P2O7+Aq.    (Stromeyer.) 

Bismuth   sodium  pyrophosphate,    NaBiP2O7 

+3H2O. 
Insol.  in  H2O.     (Rosenheim,  B.  1915,  48. 

588. 

Boron  phosphate,  BPO4. 

Insol.  in  II2O.  Not  attacked  by  boiling 
alkalies.  (Meyer,  B.  22.  2919.) 


682 


PHOSPHATE,  BROMOMOLYBDENUM 


Bromomolybdenum  phosphate. 

See  under  Bromomolybdenum  comps. 

Cadmium  ^'phosphate,  Cd5(P3Oio)2. 

Insol.  in  H2O  and  acids.  (Gliihmann, 
Dissert,  1899.) 

Cadmium     te^mphosphate,    6CdO,    4P->O6+ 

1SH2O. 
Insol.  in  acids.    (Gliihmann.) 

Cadmium  metaphosphate. 

Very  sol.  in  NH4OH+Aq.  (Persoz,  A.  ch. 
56.334.) 

Cadmium  dimetaphosphate,  Cd(PO3)^+2H2O. 
Sol.  in  32  pts.  H2O.    Scarcely  attacked  by 
acids,     especially    cone.    H2SO4.       (Glatzel, 
Dissert.  1880.) 

Cadmium  te^rawefaphosphate. 

Insol.  in  H2O.  Easily  decomp.  by  Na2S  + 
Aq.  (Fleitmann,  Poggf  73.  358.) 

Cd2(PO3)4+10H2Or  Not  so  very  difficultly 
attacked  by  acids  but  insol.  after  ignition. 
(Glatzel,  Dissert.  1880.) 


Cadmium  or^ophosphate,  Cds(PO4)2. 

Ppt.  Insol.  in  H2O.  Sol.  in  Cd  salts +Aq. 
(Stromeyer.) 

Easily  sol.  in  NH4  sulphate,  chloride, 
nitrate,  or  succinate+Aq.  (Wittstein,  Repert. 
57.  32.) 

H2Cd5(PO4)4+4H2O.  Sol.  in  dil.  H3PO4+ 
Aq.  (de  Schulten,  Bull.  Soc.  (3)  1.  473.) 

Cadmium  ZeZrahydrogen  phosphate, 

CdH4(PO4)2+2H2O. 

Decomp.  by  great  excess  of  H2O.  (de 
Schulten.) 

Cadmium  p?/r-0phosphate,  Cd2P2O7+2H2O. 

Insol.  in  H2O.  Sol.  in  NH4OH,  Na4P2O7  + 
Aq,  or  acids.  Insol.  in  KOH+Aq.  Sol.  in 
SO2+Aq.  (Schwarzenberg,  A.  65.  183.) 

Cadmium   hydrogen  or^ophosphate    hydra- 


zine 


ti   nydroge 
,  CdHPO4, 


2N2H4. 


Decomp.    by  light.      (Franzen,    Z.    anorg. 
1908,  60.  283.) 

Cadmium  potassium  te/rawetaphosphate, 

CdK3(PO3)4+3H2O. 

Sol.  in  135  pts.  H2O.    Difficultly  decomp. 
by  acids.    (Glatzel,  Dissert.  1880.) 

Cadmium  potassium  or^iophosphate. 

CdKP04. 

Insol.  in  H2O;  sol.  in  dil.  HCl+Aq.    (Ouv- 
rard,  A.  ch.  (6)  16.  321.) 


Cadmium  potassium  p?/rophosphate, 
CdK2P2O7. 

Insol.  in  H2O;  sol.  in  dil.  HCl+Aq.  (Ouv- 
rard.) 

5Cd2P2O7,  4K4P2O7+30H2O.  Much  more 
easily  sol.  in  H2O  than  the  CdNa  salt.  (Pahl, 
Sv.  V.  A.  F.  30,  7.  39.) 

Cadmium  sodium  ^riphosphate,  Na3CdP3Oio 

+  12H2O. 

Sol.  in  acids  even  after  ignition.  (Gliih- 
mann, Dissert.  1899.) 

Cadmium  sodium  /n'metaphosphate, 

Na4Cd(PO3)6+4H2O. 

SI.  sol.  in  H2O.  Insol.  in  alcohol.  (Wiesler, 
Z.  anorg.  1901,  28.  204.) 

Cadmium  sodium  tetrametaphosphate, 

Na2Cd(PO3)4+3H2O. 

Completely  insol.  in  H2O.  (Glatzel,  Dis- 
sert. 1880.) 

Cadmium  sodium  or/^ophosphate, 

CdNa4(PO4)2. 

Insol.  in  H2O;  very  sol.  in  dil.  acids. 
CdNaPO4.    As  above.    (Ouvrard.) 

Cadmium  sodium  pyro phosphate, 
CdNa2P2O7. 

Sol.  in  dil.  acids,  even  acetic  acid.  (Wall- 
roth.) 

+4H20.  Insol.  in  H2O.  (Pahl,  Sv.  V.  A. 
F.  30,  7.  39.) 

Cadmium   phosphate   bromide,    3Cd3(PO4)2, 

CdBr2. 

Sol.  in  cold  very  dil.  HN03+Aq.  (de 
Schulten,  Bull.  Soc,  (3)  1.  472.) 

Cadmium   phosphate   chloride,   3Cd3(PO4)2, 

CdCl2. 
Sol.  in  dil.  HNO3  +  Aq.    (de  Schulten.) 

Caesium  raetaphosphate,  CsPO3. 

Sol.  in  H2O.    (von  Berg,  B.  1901,  34.  4185.) 

Caesium  orZftophosphate,  Cs3PO4+5H2O. 
Deliquescent ;  very  sol .  in  H2O .    (von  Berg.) 

Caesium  hydrogen  or^/iophosphate,  Cs2HPO4 

+H2O. 
Very  sol.  in  H2O.     (von  Berg.) 

Ccesium   rf^hydrogen   or^ophosphate, 

CsH2PO4. 
Sol.  in  H2O;  insol.  in  alcohol,    (von  Berg.) 

Cesium  pyrophosphate,  Cs4P2O7. 

Very  sol.  in  H2O;  very  hydroscopic.  (von 
Berg.) 


PHOSPHATES,  CALCIUM 


683 


Calcium  /riphosphate,  5CaO,  3P2O5. 

Insol.  in  H2O.  (Schwarz,  Z.  anora.  1895, 
9.  264.) 

Calcium  monometaphosphatet  Ca(PO3)2. 

Insol.  in  H2O  and  dil.  acids.  (Maddrell,  A. 
61.  61.) 

Not  decomp.  by  digestion  with  alkali  car- 
bonates +Aq.  (Fleitmann.) 

Calcium  dimetaphosphate,  Ca2(P2O6)2  + 

4H2O. 

Insol.  in  H2O.  Decomp.  by  warm  H2SO4, 
but  not  appreciably  by  cone.  HC1  or  HNO3  + 
Aq.  (Fleitmann,  Pogg.  78.  255.) 

Calcium  hexametaph.ospha.te  (?). 

Insol.  in  H2O.  Sol.  in  Na6P6Oi8+Aq  and 
in  HCl+Aq.  (Rose,  Pogg.  76.  3.) 

Ca3P6Oi8.  Nearly  insol.  in  H2O;  sol.  in  dil. 
acids.  (Liidert,  Z.  anorg.  5.  15.) 

Calcium  or/Aophosphate,  basic,  3Ca3(PO4%  + 

CaO2H2. 

(Warington,  J.  B.  1873.  253.) 
4CaO,  P2O5.    (Hilgenstock.) 

Calcium  or^Aophosphates, 


Solubility  of  CaO  in  P2O5+Aq  at  25°. 

g.  CaO  per  1. 
of  solution 

g.  PsOsperl. 
of  solution 

Solid  phase 

7  61 

19.96 

6.51 

16.52 

5.01 

12.82 

CaHP04 

3.42 

8.16 

2.42 

5.75 

1.58 

3.66 

0.544 

1.516 

0.400 

1.108 

0.291 

0.773 

Solid  phases  are 

0.232 

0.662 

evidently  solid 

0.145 

0.381 

solutions 

0.062 

0.109 

0.049 

0.088 

0.034 

0.015 

Ca3(PO4)2 

0.587 

0.013 

\  Solid  phase  is  prob- 

0.789 

0.012 

j  ably  a  solid  solution 

(Cameron  and  Seidell,  J.  Am.  Chem.  Soc. 
1905,  27.  1513.) 


Solubility  of  CaO  in  P2O5+Aq  at  50.7°. 


Solubility  of  CaO  in  P2O5+Aq  at  25°. 

100  g.  of  the  solution 
contain 

Solid  phase 

g.  CaO  per  1. 
of  solution 

g.  P2O5  per  1. 
of  solution 

Solid  phase 

g.  P206 

g.  CaO 

> 

62.01 

0.336 

CaH4P2O8+CaH4P2O8,  H2O 

1.71 

4.69 

58.08 

0.635 

CaH4P2Os,  H20 

7.48 

22.39 

54.67 

0.939 

>< 

8.10 

23.37 

50.25 

1.428 

II 

11.57 

36.14 

46  15 

2.100 

•< 

12.88 

41.24 

41.92 

2.974 

.< 

18.77 

59.35 

37.33 

3.898 

0 

19.25 

63.03 

33  18 

4.880 

II 

23.31 

75.95 

CaHPO4,  2H2O 

29.61 

5.725 

CaH4P208,  H20  +CaHPOi 

23.69 

79.10 

15.48 

3.507 

CaHPO4 

32.41 

109.8 

9.465 

2.328 

35.90 

129.8 

6.157 

1.563 

» 

39.81 

139.6 

2.946 

0.852 

•• 

40.89 

142.7 

2.281 

0.692 

<> 

43.82 

154.6 

0.1521 

0.0588 

•« 

49.76 

191.0 

0.1527 

0.0596 

CaHPO4,  2H2O 

55.52 

216.5 

0.1331 

0.0514 

Ca3P20S)  H20. 

59.40 

234.6 

0.0942 

0.0351 

70.31 

279.7 

0.0309 

0.0106 

«« 

72.30 

fiQ   ^ 

351.9 

OfM       1 

• 

0.00068 

0.00071 

" 

V)i7  .  OO 

65.46 
63.53 

OD1  .  ± 

380.3 
395.1 

(Bassett,  Z.  anorg.  1908,  69.  15.) 

59.98 

419.7 

CaH4(PO4)2,  H2O 

59.25 

424.6 

57.74 

428.0 

53.59 

451.7 

48.78 

475.3 

44.52 

505.8 

41.86 

528.9 

» 

39.89 

538.3 

(Cameron  and  Seidell,  J.  Am.  Chem.  Soc. 

1905,  27.  1508.) 

684 


PHOSPHATE,  CALCIUM 


Solubility  of  CaO  in  P2O5+Aq  at  40°. 

100  g.  of  the  solution 

contain 

Solid  phase 

g.  P205 

g.  CaO 

45.42 

1.768 

CaH4P2O8,  H2O 

41.33 

2.588 

u 

36.79 

3.584 

u 

32.46 

4.505 

(c 

28.27 

5.501 

" 

21.67 

4.813 

CaHP04 

17.78 

4.100 

" 

16.35 

3.810 

K 

9.905 

2.536 

n 

6.979 

1.847 

<( 

4.397 

1.267 

ce 

1.819 

0.576 

(i 

0.423 

0.156 

u 

0.294 

0.110 

(( 

0.158 

0.0592 

a 

0.146 

0.0519 

u 

0.128 

0.0508 

Ca3P208,  H2O 

0.0262 

0.0098 

u 

trace 

0.0709 

Ca4P2O9,  4H2O 

u 

0.0814 

it 

ti 

0.0829 

« 

se 

0.0840 

ee 

(Bassett,  Z.  anorg.  1908,  59.  18.) 

Solubility  of  CaO  in  P2O5-fAq  at  25°. 

100  g.  the  solution 

contain 

Solid  phase 

g.  PsOs 

g.  CaO 

36.11 

3.088 

CaH4P2O8,  H2O 

31.97 

4.128 

« 

28.34 

4.908 

ii 

27.99 

4.930 

it 

25.45 

5.489 

11 

22.90 

5.523 

CaHPO4 

17.55 

4.499 

" 

15.34 

4.027 

« 

9.10 

2.638 

u 

6.049 

1.878 

a 

3.613 

1.181 

(t 

2.387 

0.826 

a 

0.417 

0.165 

CaHPO4+CaHPO4,  2H2O 

0.178 

0.0696 

(( 

0.0332 

0.0126 

u 

0.0948 

0.0352 

Probably  Ca3P2Os,  H2O 

0.0571 

0.0211 

a 

0.0525 

0.0175 

M 

0.0468 

0.0186 

11 

trace 

0.1131 

Ca4P209,4H20+Ca(OH)2 

0.118 

Ca(OH)2 

(Bassett,  Z.  anorg.  1908,  59.  20.) 

Calcium  or^ophosphate,  Ca3(PO4)2. 

Decomp.  by  long  boiling  with  H2O  into 
basic  salt,   3Ca3(PO4)2,   CaO2H2.     This  de- 
comp.  begins  with  cold  H2O,  so  that  the  solu 
bility  at  6-8°  varies  from  9.9  to  28.6  mg.  in  a 
litre^    (Warington,  Chem.  Soc.  (2)  11.  983.) 


1  1.  cold  H2O  dissolves  in  7  days  31  mg. 
gnited,    and    79    mg.    freshly    precipitated 
Ca3(PO4)2.    (Volcker,  J.  B.  1862.  131.) 

100,000  pts.  H2O  dissolve  2.36  pts.  gelatin- 
ous Ca  phosphate;  2.56  pts.  ignited  Ca  phos- 
)hate;  3.00  pts.  Ca  phosphate  from  bone  dust. 
Maly  and  Donath,  J.  pr.  (2)  7.  416.) 

Solubility  of  bones  in  various  solvents  is 
given  bv  Maly  and  Donath,  I.  c. 

0.009"  g.    Ca3(PO4)2  is  sol.  in   1  1.  H2O. 

0.153    "          "  "     "     "      " 

sat.  with  CO2.     (Joffre,  Bull.  Soc.  1898,  (3) 
19.372.) 

Determinations  of  solubility  in  H2O  as 
stated  in  the  literature  vary  because  Ca3(PO4)2 
s  apparently  a  solid  solution  of  CaHPO4  and 
UaO.  When  placed  in  contact  with  H2O 
more  PO4  ions  dissolve  than  Ca  ions,  the 
resulting  solution  is  acid  and  solid  phase 
•icher  in  Ca  than  before  addition  of  H2O. 
For  material  of  the  approximate  composition, 

a3(PO4)2,  the  amt.  dissolved  by  CO2  free  H2O 
at  ord.  temp,  is  0.01-0.10  g.  per  1.  depending 
on  conditions  of  experiment.  H2O  sat  with 

02  dissolves  0.15-0.30  g.  per  1.    (Cameron 
and  Hurst,    J.  Am.   Chem.   Soc.    1904,   26. 
903.) 

The  decomposition  of  Ca3(PO4)2  in  H2O  is 
increased  by  presence  of  CaSO4;  decreased  by 
presence  of  CaCO3  or  of  CaSO4  and  CO2.  CO2 
increases  the  amount  of  PO4  dissolved  in  the 
solution  of  water  alone  and  the  sat.  CaSO4 
solutions,  but  has  no  other  effect  than  to  in- 
crease the  amount  of  Ca  in  the  solutions  in 
contact  with  CaCO3.  (Cameron  and  Seidell, 
J.  Am.  Chem.  Soc,  1904,  26.  1458.) 

Sol.  in  CO2+Aq. 

1  1.  H2O  containing  1  vol.  CO2  dissolves  in 
12  hours  at  10°  0.75  g.  precipitated  Ca3(PO4)2; 
0.166  g.  Ca3(PO4)2  from  bone  ash;  0.300  g. 
Ca3(PO4)2  from  bones  which  had  been  buried 
20  years.  (Lassaigne,  J.  ch.  me"d.  (3)  3.  11.) 

1  1.  H2O  containing  0.8  vol.  CO2  dissolves 
0.61  g.  Ca3(PO4)2.  (Liebig,  A.  106.  196.) 

H2O  sat.  with  CO2  at  5-10°  and  760  mm. 
pressure  dissolves  0.527-0.60  g.  Ca3(PO4)2,  or, 
if  containing  1%  NH4C1,  0.739  g.  Ca3(PO4)2. 
(Warington,  Chem.  Soc.  (2)  9.  80.) 

Solubility  varies  according  to  form  of 
Ca3(PO4)2/ 

In  apatite,  1  pt.  Ca3(PO4)2  dissolves  in 
222.222  pts.  H2O  sat.  with  CO2;  in  raw  bones, 
in*  5698  pts.;  in  bone  ash,  in  8029  pts.;  in 
So.  Carolina  phosphate,  in  6983  pts.;  in  phos- 
phatic  guano  from  Orchilla  Id.,  in  8009  pts. 
(Williams,  C.  N.  24.  306.) 

A12O6H6  and  Fe2O6H6  prevent  the  solubility 
of  Ca3(PO4)2  in  H2O  containing  CO2.  (War- 
ington, I.  c.} 

1  1.  H2O  dissolves  0.22848  g.  Ca3(PO4)2. 
under  a  CO2-pressure  of  2  atmos.  at  14°. 
(Ehlert,  Z.  Elektrochem.  1912,  18.  728.) 

Sol.  in  S02+Aq,  forming  a  liquid  of  1.3  sp. 
gr.  at  9°  from  freshly  precipitated  Ca3(PO4)2, 
and  of  1.188  sp.  gr.  from  bone  ash. 

Sol.  in  H2S+Aq.     1  1.  H2O  sat.  with  H2S 


PHOSPHATE,  CALCIUM 


685 


dissolves  190-240  mg.  Ca3(PO4)2.    (Bechamp, 
A.  ch.  (4)  16.  241.) 

Easily  sol.  in  HNO3  or  HCl+Aq. 

100  pts.  very  dil.  HCl+Aq  dissolve  198-225 
pts.  Ca3(PO4)2.    (Crum,  A.  63.  294.) 

100  pts.  HC1  of  1.153  sp.  gr.  (containing 
31%  HC1)  dissolve  at  17°  when  diluted  with: 

0147    pts.  H2O, 
25.3        45.0        62.3        64.7  pts.  Ca3(PO4)2, 

10  13  16  19    pts.  H2O. 

68.0        71.9        69.5        69.7  pts.  Ca3(PO4)2. 
(Bischof,  Schw.  J.  67.  39.) 

Decomp.  by  H2SO4. 

Completely  decomp.  to  CaSO4  and  H3PO4 
by  a  mixture  of  H2SO4  and  alcohol. 

Solubility  in  HNO3+Aq. 

1  pt.  of  Ca3(PO4)2  dissolves  at  16.25-17.5°  in 
pts.  HNOs+Aq  which  contain  pts.  H2O 
to  1  pt.  HNO3  (sp.  gr.  =  1 .23). 


Dry  Ca3(PO<i)2  also  dissolves  by  long  boiling 
with  solutions  of  ammonium  chloride,  nitrate, 
succinate  (Wittstein),  or  sulphate  (Delkes- 
kamp). 

Sol.  in  89,448  pts.  H2O  (boiled)  at  7°; 
19,628  pts.  H2O  (boiled)  containing  1% 
NH4C1  at  10°;  4324  pts.  H->O  (boiled)  con- 
taining 10%  NH4C1  at  17°;  1788  pts.  H2O  sat. 
with  CO2  and  containing  10%  NH4C1  at  10° 
and  751  mm.  pressure;  1351  pts.  H2O  sat. 
with  CO2  and  containing  1%  NH4C1  at  12° 
and  745  mm.  pressure;  42,313  pts.  H2O  sat. 
with  CO2  and  containing  CaCO3  at  21°  and 
756.3  mm.  pressure;  18,551  pts.  HoO  sat.  with 
CO2  and  containing  CaCO3  and  1%  NH4C1  at 
16°  and  746.1  mm.  pressure.  (Warington, 
Chem.  Soc.  (2)  4.  296.) 

Aqueous  solutions  of  the  following  NH4 
salts  dissolve  the  given  amts.  of  Ca3(PO4)2, 
calculated  for  100  pts.  of  the  corresponding 
acid:  NH4C1,  0.655  pt.;  NH4NO3,  0.306  pt.; 


Pts. 
HNOs+Aq 

Pts.  H20 

Pts. 
HNOs+Aq 

Pts.  H2O 

(,iNn4;2i5U4,  i.uou  pts.;  i\n4^2jn3vj2,  u.zoo  pt.; 
NH4  tartrate,  4.56  pts.;  NH4  citrate,  7.015 
pts.;  NH4  malate,  1.125  pts.  Ca3(PO4)2.  (Ter- 
reil,  Bull.  Soc.  (2)  35.  578.) 

Solubility  in  various  salts  +Aq  under  a  CO2 
pressure  of  2  atmospheres,  at  14°. 

2.72 
4.23 
10.25 
15.45 
20.34 
20.82 

0 
0.827 
3.309 
5.791 

8.273 
10 

30.64 
26.48 
32.14 
36.06 
127.81 

10.754 
13 
13.236 
15.718 
40 

Salt 

G.  salt  per 
100  g.  H2O 

G.  Cas(PO4)2 
sol.  in  1  1.  of  the 
solvent. 

(Bischof,  1833.) 

More  sol.  in  acetic,  lactic,  malic,  and  tar- 
taric    acids    than    in    HC1    or    HNO3+Aq. 
(Crum.) 
Solubility  in  H3PO4-f  Aq. 

H20 

0.22848 

NaCl 

50 
cone. 

1.3208 
0.64089 

G.  HsPO4 
HaPO 

n  100  cc.  of 
4+Aq 

G.  Ca3(PO4)2  dissolved 
by  100  cc.  of  solvent 

MgCl2+6H2O 

86.9 
cone. 

1.2873 
2.8923 

5 

10 
15 
20 
25 
30 

3.85 
7.28 
9.45 
12.50 
13.79 
15.10 

KMgCl3+6H2O 

79.2 
cone. 

1.5771 
1.1536 

K2S04,MgS04, 
MgCl2+6H2O 

70.95 
cone. 

1.7777 
2.4911 

NaN03 

72.7 
cone. 

1.5827 
0.8638 

(Causse,  C.  K.  1892,  114.  414.) 

Very  small  quantities  of  the  salts  of  the 
alkali  metals  increase  the  solubility  in  H2O. 
(Lassaigne,  J.  chim.  med.  (3)  3.  11.) 
1  litre  cold  HoO  with  2  g.  NaCl  dissolves 
45.7  mg.  Ca3(PO4)2;  with  3  g.  NaNO3,  33  mg. 
Ca3(P04)2.    (Liebig.) 
1  litre  H2O  containing  8.75%  NaCl  dissolves 
317.5  mg.  Ca(PO4)2.    (Lassaigne.) 
NH4  salts  have  even  more  effect,  especiallv 
NH4Cl+Aq,   which   dissolves   Ca3(PO4)2  in 
the  cold;   also  ammonium  nitrate  and  suc- 
cinate.    (Wittstein.) 
(NH4)2SO4+Aq    dissolves    Ca3(PO4)2    as 
easily  as  CaSO4.    (Liebig,  A.  61.  128.) 
1  litre  H2O  containing  2  g.  NaCl  dissolves 
at  7-12.3°  45.7  mg.  Ca3(PO4)2;  3  g.  NaNO3 
at  17.3°,  33  rng.  Ca3(PO4)2;  2.2  g.  (NH4)2SO4, 
76.7  mg.  Ca3(PO4)2.    (Liebig,  A.  106.  185.) 

K2S04 

74.5 
cone. 

4.9041 
4.7649 

(NH4)2S04 

56.5 
cone. 

2.4131 

5.8849 

Na2SO4+10H2O 

137.7 
cone. 

2.4911 
3.2267 

MgSO4+7H2O 

105.3 
cone. 

1.9728 
3.6001 

NH4C1 

45.74 
cone. 

1.3710 
1.2929 

(Ehlert  and  Hempel,  Z.  Elektrochem.  1912, 
18.  728.) 

686 


PHOSPHATE,  CALCIUM 


Ca3fPO4)2  is  sol.  in  K2C2O4+Aq.  100  ccm. 
K2C2O4+Aq  (iy2%  K2C2O4)  dissolves  57.1% 
of  the  P2O5  from  phosphorite,  71  %  from  guano 
by  boiling  25  min.  At  ord.  temp,  bone  meal 
gives  up  50-80%  of  its  P2O5  to  K2C2O4+Aq 
in  36  hours.  (Liebig,  Landw.  J.  B.  1881.  603.) 

Sol.  in  Ca  suorate+Aq.  (Bobierre,  C.  R. 
32.  859.) 

More  sol.  in  H2O  containing  starch,  glue,  or 
other  animal  substances  than  in  pure  H2O. 
(Vauquelin,  Pogg.  85.  126.) 

Sol.  in  H2O  containing  organic  matter, 
therefore  when  bones  decay  under  H2O, 
Ca3(PO4)o  is  dissolved  in  considerable  quan- 
tity. (Hayes,  Edin.  Phil.  J.  5.  378.) 

Sol.  in  sodium  citrate  +Aq.    (Spiller.) 

Solubility  in  NH4  citrates +Aq. 

Ammonium  citrate  solution  of  1.09  sp.  gr. 
at  30-35°  dissolves  precipitated  Ca3(PO4)2 
completely,  but  not  phosphorite.  (Frese- 
nius.) 

Dried  on  the  oir,  with  2V&H2O.  Sol.  in  40 
min.  in  diammonium  citrate+Aq  (sp.  gr.  = 
1.09);  triammonium  citrate+Aq  (sp.  gr.  = 


1.09)  dissolves  55.3%  of  the  P,O5;  citric  acid 
+Aq  (H%)  dissolves  83.8%  of  the  P2O5. 
(Erlenmeyer,  B.  14.  1253.) 

Dried  at  50°,  with  17/8H2O.  Sol.  in  45  min. 
in  diammonium  citrate+Aq  (sp.  gr.  =  1.09); 
triammonium  citrate+Aq  dissolves  52.3%  of 
the  P2O5.  (Erlenmeyer.) 

Ignited.  Diammonium  citrate+Aq  (sp.  gr. 
1.09)  dissolves  93%  of  the  P2O5;  triammonium 
citrate+Aq  (sp.  gr.  1.09)  dissolves  32%  of  the 
P2O5;  citric  acid  (M%)  dissolves  53.4%  of 
the  P2O8.  (Erlenmeyer.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Insol.  in  alcohol  and  ether. 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 

Min.  Apatite. 

0.002  g.  is  sol.  in  1  1.  H2O. 

0.014  "  "  "  "  1  1.  H2O  sat.  with  CO2. 
(Joffre,  Bull.  Soc.  1898,  (3)  19.  374.) 


+H2O.    Solubility  in  H2O,  in  H2O  sat.  with  CO2,  and  in  H2O  containing  CO2+CaH2(CO3)2. 

Temp.  16°-20°. 


ooiveut 

P2O5  mg. 

CaO  mg. 

(1)  Boiled  distilled  H2O. 

0.74 

(2)  1200  cc.  distilled  H2O+50  cc.  H2O  sat. 

with  CO2. 

6.9 

(3)  1000  cc.       "            "  +250  cc.  "      " 

tt      tt 

48.5 

(4)  1250  cc.  H2O  sat.  with  CO2. 

91.9 

Solutions  of  CO2+CaH2(CO3)2.    1  1. 

(filtered)  contains: 

Calcium  carbonate 

13  mg. 

(5)   j 

Bicarbonate             j  g±£facid 

166    ' 
73    ' 

0.38 

100.0 

Free  carbonic  acid 

9    ' 

Calcium  carbonate 

13    ' 

(6) 

Bicarbonate             {  g±£facid 

277    ' 
122    " 

1.1 

162.3 

Free  carbonic  acid 

49    " 

Calcium  carbonate 

13    " 

(7) 

Bicarbonate              ^  v^aroonate 

376    " 
165    " 

0.80 

218.8 

Free  carbonic  acid 

105    " 

Calcium  carbonate 

13    " 

(8) 

Bicarbonate            {  g^^cacid 

475    " 
209    " 

1.77 

273.3 

Free  carbonic  acid 

206    " 

Calcium  carbonate 

13    " 

(9) 

-DlCcWDOIlSlt/G                   "{    /~*\      i         •           »i 

545    " 
240    " 

1.30 

312.7 

Free  carbonic  acid 

301    " 

In  1  1.  of  the  filtrate 


(Schloesing,  C.  R.  1900,  131.  151.) 


PHOSPHATE,  CALCIUM  HYDROGEN 


687 


Calcium  hydrogen  phosphate.  CaHPO4,  and 
+2H20. 

Insol.  or  nearly  so  in  H2O.  Gradually 
decomp.  by  cold,  more  quickly  by  hot  H2O. 

1000  pts.  H2O  dissolve  0.135-0.152  pt. 
CaHPO4+2H2O.  Solution  clouds  up  on  boil- 
ing. (Birnbaum.) 

1000  pts.  H2O  dissolve  0.28  pt.,  and  if  sat. 
with  CO2,  0.66  pt.  CaHPO4+2H2O.  (Dusart 
and  Pelouze.) 

When  this  salt  dissolves  in  H2O,  decomp. 
takes  place  and  a  very  considerable  time  is 
necessary  to  establish  equilibrium.  (Rindell, 
C.  R.  1902,  134.  112.) 

Much  less  decomp.  by  H2O  than  Ca3(PO4)2 
or  CaH4(PO4)2,  and  the  decomposition  of 
this  salt  in  water  depends  only  slightly  upon 
the  relative  amounts  of  solid  and  solvent 
which  are  present.  The  decomposition  is  in- 
creased by  the  addition  of  CO2.  The  presence 
of  CaSO4  or  of  CaCO3  decreased  the  amount 
of  phosphoric  acid  which  dissolved.  See 
original  paper.  (Cameron  and  Seidell,  J.  Am. 
Chem.  Soc,  1904,  26.  1460.) 

When  the  ratio  of  P2O5  :  CaO  is  above  1.0 
or  below  1.27,  H2O  dissolves  0.4CK).54  g.  CaO 
and  1.11-1.52  g.  P2O5  (see  original  paper). 
(Cameron  and  Bell,  J.  Am.  Chem.  Soc.  1905, 
27.  1512.) 

Solubility  in  H3PO4+Aq. 


G.  H3PO4  in  100  cc. 
H3PO4+Aq 

G.  CaHPO4  dissolved  by 
100  cc.  of  solvent 

5 

4.30 

10 

7.15 

15 

9.30 

20 

11.86 

25 

13.40 

30 

15.10 

(Causse,  C.  R.  1892,  114.  415.) 

1  1.  H2O  containing  2.2  g.  (NH4)2SO4,  2  g. 
NaCl,  or  3  g.  NaNO3  dissolves  79.2,  66.3,  or 
78.9  mg.  CaP2O7,  which  is  present  in  form  of 
CaHPO4.  (Liebig,  A.  106.  185.)  Slowly  but 
completely  sol.  in  boiling  NH4Cl+Aq. 
(Kraut,  Arch.  Pharm.  (2)  111.  102.)  Easily 
sol.  in  H2SO3+Aq.  (Gerland,  J.  pr.  (2)  4. 
123.)  Very  sol.  in  HC1  or  HNO3+Aq.  Less 
sol.  in  HC2H3O2.  (Berzelius.)  More  sol.  in 
dil.  than  cone.  HC2H3O2+Aq,  but  60  pts. 
HC2H3O2  (1  mol.)  dissolve  at  most  23.1  pts. 
P2O5  (1  mol.  =  142  pts.)  from  this  compound. 
Aqueous  solution  of  sodium  acetate  dissolves 
more  easily  than  H2O,  and  becomes  turbid 
on  boiling.  (Birnbaum.) 

Completely  sol.  in  K2C2O4+Aq.  (Liebig, 
Landw.  J.  B.  1881.  603.) 

1 1.  of  sat.  solution  in  N/200  acid  K  tartrate 
+Aq  at  25°  contains  0.235  g.  CaHPO4. 

Insol.  in  alcohol.  Sol.  in  many  organic 
substances,  as  starch  or  gelatine +Aq. 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014.) 


+  V3H2O.  (Vorbringer,  Z.  anal.  9.  457.) 

+H2O.    (Gerlach,  J.  pr.  (2)  4.  104.) 

+2H2O.    Min.  Brushite. 

+3H2O.    Min.  Metabrushite. 

+  5H2O.    (Dusart,  C.  R.  66.  327.) 


Calcium  tetrahydrogen  or^Aophosphate, 
CaH4(P04)2+H20. 

Very  deliquescent.  Crystals  take  up  97.7 
pts.  H2O  in  16  days,  and  226  pts.  H2O  in  28 
days  from  air  saturated  with  moisture. 
(Birnbaum,  Zeit.  Ch.  (2)  7.  131.) 

Not  hygroscopic  when  pure.     (Stocklasa, 

B.  23.  626  R.) 

Completely  sol.  in  100  pts.  H2O,  but  de- 
comp. by  10-40  pts.  H2O  with  separation  of 
CaHPO4,  which  slowly  dissolves.  (Erlen- 
meyer,  J.  B.  1873.  254.) 

Later  (B.  9.  1839)  Erlenmeyer  says 
CaH4(PO4)2+H2O  is  sol.  in  700  pts.  H2O  and 
decomp.  into  CaHPO4  by  a  less  amount  of 
H2O.  Wattenberg  (Z.  anal.  19.  243)  says  that 
the  decomposition  by  small  amts.  of  H2O 
down  to  144  pts.  H2O  to  1  pt.  salt  is  inappre- 
ciable. 

Completely  sol.  in  200  pts.  H2O  if  pure,  and 
in  less  H2O  in  presence  of  H3PO4.  (Stocklasa.) 

Sol.  in  25  pts.  H2O  at  15°.  Solution  begins 
to  decompose  when  warmed  to  50°.  (Otto, 

C.  C.  1887.  1563.) 

Greatly  decomp.  by  H2O  and  the  resulting 
solution  is  to  be  regarded  as  a  solution  of  the 
decomposition  products  rather  'than  of  the 
substance  itself.  The  presence  of  an  excess 
of  CaSO4  does  not  materially  affect  the 
amount  of  phosphoric  acid  entering  the  solu- 
tion. (Cameron,  J.  Am.  Chem.  Soc.  1904,  26. 
1462.) 

Violently  decomp.  by  H2O  in  cone,  solu- 
tion; only  si.  decomp.  when  dissolved  in  200 
pts.  H2O.  (Stocklasa,  Z.  anorg.  1892,  1.  310.) 

Solubility  of  CaH4P2O8  in  H3PO4+Aq  at 
pressure  of  745  mm.  at  high  temp. 


ft 
PP 

100  g. 
of  the  solution 
contain 

Solid  phase 

G. 
P205 

G. 

CaO 

115° 
132° 
169° 

43.60 
53.43 
63.95 

5.623 
4.327 

4.489 

CaH4P208,  H2O+CaHPO4 
CaH4P2O8+CaH4P2O8,  H2O 
CaH^Os 

(Bassett,  Z.  anorg.  1908,  69.  26.) 

Glacial  HC2H3O2  ppts.  it  completely  from 
aqueous  solution  even  in  presence  of  HNO3. 
(Persoz.) 

Decomp.  by  50  pts.  absolute  alcohol  at  b.- 
pt.  in  1  hour;  by  30  pts.  in  2  hours.  Sol.  in 
absolute  ether.  (Erlenmeyer,  I.e.) 


688 


PHOSPHATE,  CALCIUM 


Calcium  p?/rophosphate,  Ca2P2O7+4H2O. 

Somewhat  sol.  in  H2O;  completely  sol.  in 
mineral  acids;  less  sol.  in  acetic  acid,  and  in- 
sol.  in  Na4P2O7+Aq.  (Schwarzenberg,  A. 
65.  145.)  Less  sol.  in  warm  than  in  cold  acetic 
acid.  (Baer,  Pogg.  75.  155.) 

Insol.  in  NH4Cl+Aq.  (Wackenroder,  A. 
41.  316.) 

Insol.  in  CaCl2+Aq. 

Min.  Pyrophosphorite. 

Calcium  hydrogen  pz/rophosphate,  CaH2P2O7 
+2H2O. 

Sol.  in  H2O.    (Pahl,  B.  7.  478.) 

2CaH2P2O7,  Ca?P2O7+6H2O.  Decomp.  by 
boiling  with  H2O  into — 

CaIi2P2O7,  Ca2P2O7+3H2O.  Insol.  in  hot 
H2O.  (Knorre  and  Oppelt,  B.  21.  771.) 

Tefracalcium  hydrogen  phosphate, 
Ca4H(P04)3+H20. 

Ppt.  Insol.  in  H2O,  but  decomp.  by  boiling 
therewith.  Sol.  in  acids.  (Warington, 
Chem.  Soc.  (2)  4.  296.) 

+2H2O. 

Calcium  tefraphosphate,  Ca3P4O13. 

Insol.  in  acids  when  ignited.  (Fleitmann 
and  Henneberg,  A.  65.  331.)  • 

Calcium  lithium  phosphate,  CaLiPO4. 
Insol.  in  H;2O.    (Rose,  Pogg.  77.  298.) 

Calcium  potassium  cfo'raefaphosphate, 

CaK2(P2O6)2+4H2O. 
As  BaK  comp.    (Glatzel,  Dissert.  1880.) 

Calcium  potassium  or/ftophosphate,  CaKPO4. 
Insol.  in  H2O.    (Rose,  Pogg.  77.  291.) 
Easily  sol.  in  acids.     (Ouvrard,  A.  ch.  (6) 

16.  308.) 

Calcium  potassium  p^/rophosphate,  CaK2P2O7. 
Insol.   in   H2O;    easily  sol.   in   dil.    acids. 
(Ouvrard,  C.  R.  106.  1599.) 

Calcium  sodium  dimetaphosphate, 

CaNa2(P2O6)2+4H2O. 
As  BaNa  comp.    (Glatzel.) 

Calcium  sodium  Znwetaphosphate, 

CaNaP3O9+3H2O. 

SI.  sol.  in  H2O.    (Fleitmann,  A.  65.  315.) 
Easily  sol.  in  H2O.    Difficultly  sol.  in  HCI+ 

Aq  when  heated  to  redness.     Easily  sol.  in 

boiling  HCl+Aq  after  being  fused.     (Lind- 

bom.) 

Calcium  sodium  or^/iophosphate,  CaNaPO4. 
Insol.  in  H2O.    (Rose,  Pogg.  77.  292.) 
Easily  sol.  in  dil.  acids.     (Ouvrard,  A.  ch. 

(6)  16.  308.) 
3CaO,  3Na2O,  2P2O5.     Sol.  in  dil.  acids. 

(Ouvrard,  C.  R.  1888,  106.  1599.) 


Calcium  sodium  p?/rophosphate,  CaNa2P2O7 
+4H2O. 

Insol.  in  Na4P2O7+Aq.  Easily  sol.  in 
IICl+Aq,  HNO3+Aq,  and  also  in  HC2H3O2 
+Aq.  (Baer,  Pogg.  75.  159.) 

Ca10Nai6(P2O7)9.  Sol.  in  acids.  (Wallroth, 
Bull.  Soc.  (2)  39.  316.) 

3CaO,  3Na2O,  2P2O5.  Easily  sol.  in  acids. 
(Ouvrard,  A.  ch.  (6)  16.  307.) 

Calcium  thorium  raetaphosphate,  ThO2.  CaO, 

P205. 
(Colani,  C.  R,  1909,  149.  209.) 

Calcium  uranous  raetaphosphate,  UO2,  CaO, 

P205. 

Insol.  in  acids.  (Colani,  A.  ch.  1907,  (8) 
12.  140.) 

Calcium  uranyl  phosphate,  Ca(UO2)H2(PO4)2 
+2,  3,  or  4H2O. 

Sol.  in  HNO3+Aq.    (Debray.) 

Ca(UO2)o(PO4)2+8H2O.  Min.  Uranite. 
Sol.  in  HNO3+Aq. 

3CaO,  5UO3,  2P206+16H2O.  (Blinkoff, 
Dissert.  1900.) 

Calcium  phosphate  chloride,  Ca3(PO4)2,  CaCl2. 

(Deville  and  Caron,  A.  ch.  (3)  67.  458.) 

3Ca3(P04)2,  CaCl2.  Chlor apatite.  Insol.  in 
H20.  (Daubree,  Ann.  Min.  (4)  19.  684.) 

7CaH4(PO4)2,  CaCl2+14H2O.  Sol  in 
HCl+Aq. 

4CaH4(PO4)2,  CaCl.+SHsO. 

CaH4(PO4)o,  CaCl2+2H2O.  Partly  sol.  in 
H2O  with  decomp.  Also  with  8H2O.  (Erlen- 
meyer,  J.  B.  1857.  145.) 

Calcium  phosphate  chloride  fluoride, 

3Ca3(PO4)2,  CaClF. 

Min.  Apatite.  Boiling  H2O  dissolves  out 
CaCl2;  dil.  mineral  acids  dissolve  easily,  acetic 
acid  with  more  difficulty.  Easily  soluble  in 
molten  NaCl,  crystallizing  on  cooling.  (Forch- 
hammer.) 

Calcium    phosphate    silicate,    Ca3(PO4)2, 
Ca2SiO4. 

Insol.  in  H2O;  decomp.  by  HCl+Aq. 
(Carnot  and  Richard,  C.  R.  97.  316.) 

4Ca3(PO4)2,  Ca3SiO5.  (Bucking  and  Linck, 
C.  C.  1887.  562.) 

4Ca3(PO4)2,  3Ca3SiO5.    (B.  and  L.) 

Ca(PO3)2,  CaSiO3.  (Stead  and  Ridsdate, 
Chem.  Soc.  51.  601.) 

Calcium     dihydrogen     phosphate     sulphite, 

CaH2(PO4)2,  CaSO3+H2O. 
Not  decomp.  by  cold,  slowly  by  boiling 
H2O.  Slightly  sol.  in  NH4OH+Aq.  Sol.  in 
mineral  acids.  Insol.  in  cold,  slowly  sol.  in 
boiling  acetic  acid.  More  sol.  in  a  solution  of 
oxalic  acid.  (Gerland,  C.  N.  20.  268.) 


PHOSPHATE,  COBALTOUS 


689 


Cerous  metaphosphate,  Ce(PO3)3. 

(Rammelsberg.) 

Ce2O3,  5P2O&.  Insol.  in  H2O  or  acids. 
(Johnsson,  B.  22.  976.) 

Cerous  or^ophosphate,  CePO4. 

Insol.  in  H2O.  Easily  sol.  in  acids. 
(Grandeau,  A.  ch.  (6)  8.  193.) 

Insol.  in  acids.  (Hartley,  Proc.  Roy.  Soc. 
41.  202.) 

+2H2O.  Insol.  in  H2O.  Sol.  in  acids. 
(Jolin.) 

Insol.  in  H3PO4+Aq;  si.  sol.  in  HC1  or 
HNO3+Aq.  (Hisinger.) 

Insol.  in  HNO3+Aq.  (Boussingault,  A.  ch. 
(5)  6.  178.) 

Min.  Cryptolite.  Completely  decomp.  by 
H.2SO4  when  finely  powdered.  Insol.  in  dil. 
HNOa+Aq. 

Ceric  or^ophosphate,  4CeO2,  6P2O5+26H2O. 
Ppt.    (Hartley,  Proc.  Roy.  Soc.  41.  202.) 

Cerous  p?/rophosphate,  Ce2H2(P2O7)6+6H2O. 

Sol.  in  cerous  nitrate +Aq. 

Ce4(P2O7)3  +  12H2O.  Sol.  in  excess  of 
sodium  pyrophosphate+Aq.  Easily  sol.  in 
HC1.  (Rosenheim,  B.  1915,  48.  592.) 

Cerous  lanthanum  thorium  phosphate, 

(Ce,  La,  Th)2(PO4)2. 

Min.  Monazite.  Sol.  in  HCl+Aq  with 
white  residue. 

Cerous   potassium    orZ/iophosphate,   2Ce2O3, 
.   3K,O,  3P2O5  =  2CePO4,  K3PO4. 
Insol.  in  H2O;  sol.  in  acids.     (Ouvrard,  C. 

R.  107.  37.) 

Cerous  sodium  or^ophosphate,  Ce2O3,  3Na2O, 

2P2O5  =  CeP04,  Na3PO4. 
Insol.  in  H2O.    (Ouvrard,  C.  R.  107.  37.) 

Cerous  sodium  pyrophosphate,  CeNaP2O7. 

Insol.  in  acetic,  and  cold  dil.  mineral  acids. 
Sol.  in  warm  acids.  (Wallroth.) 

Chromous  phosphate,  Cr3(PO4)2. 

Insol.  in  H2O.  Easily  sol.  in  citric,  tartaric 
and  acetic  acids.  SI.  sol.  in  H2CO3+Aq. 
(Moissan,  A.  ch.  1882,  (5)  25.  415.) 

+H2O.  Precipitate.  Easily  sol.  in  acids. 
(Moberg;  Moissan,  A.  ch.  (5)  21.  199.) 

Chromic  wetaphosphate,  Cr2(PO3)6. 

Insol.  in  H2O  or  cone,  acids.  (Maddrell,  A. 
61.  53.) 

Chromic  ort'/iophosphate,  CrPO4. 

Hydrolyzed  by  hot  H2O.  Somewhat  sol. 
in  NH4OH+Aq  and  in  Cr2(SO4)3+Aq. 
(Caven,  J.  Soc.  Chem.  Ind.  1897/16.  29.) 

Insol.  in  methyl  acetate.     (Naumann,  B. 


1909,  42.  3790);  ethyl  acetate.     (Naumann, 
B.  1910,  43.  314.) 

Chromic  phosphate,  Cr2(PO4)2  +  12H2O. 

Violet  modification.  Precipitate.  (Ram- 
melsberg, Pogg.  68.  383.) 

-f-6H2O.  Green  modification.  Very  si. 
sol.  in  ~HoO  and  still  less  in  NH4NO3  or 
NH4C2H362+Aq.  (Carnot,  C.  R.  94.  1313.) 

Insol.  in  acetic,  but  easily  sol.  in  mineral 
acids.  Easily  sol.  in  cold  KOH  or  NaQH  + 
Aq,  from  which  it  is  separated  on  boiling. 
(Bowling  and  Plunkett,  Chem.  Gaz.  1868. 
220.) 

Chromic  hydrogen  phosphate,  Cr2H6(PO4)4+ 

16H2O. 
Sol.  in  H2O.    (Haushofer.) 

Chromic  p?/rophosphate,  Cr4(P2O7)3. 

Anhydrous.  Insol.  in  H2O  or  acids.  (Ouv- 
rard, A.  ch.  (6)  16.  344.) 

+7H2O.  Precipitate.  Sol.  in  strong 
mineral  acids,  SO2+Aq,  KOH+Aq,  and 
Na.4P2O7+Aq.  (Schwarzenberg,  A.  65.  149.) 

Insol.  in  Na4P2O7+Aq.    (Stromeyer.) 

Chromic  potassium  phosphate,  Cr2O3,  K2O, 

2P2O6. 

Insol.  in  H2O  and  in  acids.  (Ouvrard,  A. 
ch.  (6)  16.  289.) 

Chromic  potassium  p^/rophosphate, 
K(CrP2O7)+5H2O. 

SI.  sol.  in  cold  H2O.  Decomp.  by  boiling 
H2O.  (Rosenheim,  B.  1915,  48.  586.) 

Cr2K2H4(P2O7)3.  Insol.  in  H2O,  acids,  or 
alkalies.  SI.  decomp.  by  boiling  cone.  H2SO4. 
(Schjerning,  J.  pr.  (2)  45.  515.) 

Chromic   silver  phosphate,   2Cr2O3,    2Ag2O, 

5P2O5. 

(Hautefeuille  and  Margottet,  C.  R.  96. 
1142.) 

Chromic  sodium  or^ophosphate,  Na2HPO4, 

2CrPO4+5H2O. 

Decomp.  by  H2O.  (Cohen,  J.  Am.  Chem. 
Soc.  1907,  29.  1197.) 

Chromic  sodium  p«/rophosphate, 
Cr2Na2(P2O7)2. 

Insol.  in  acids.  (Wallroth,  Bull.  Soc.  (2) 
39.  316.) 

+  10H2O,  and  16H2O.  SI.  sol.  in  cold  H2O. 
Decomp.  by  boiling  H2O.  (Rosenheim,  B. 
1915,  48.  586.) 

Cobaltous  raorcoraetaphosphate,  Co(PO3)2(?). 
Insol.  in  H2O  and  dil.  acids.    Sol.  in  cone. 
HCl+Aq.    (Maddrell,  A.  58.  61.) 


690 


PHOSPHATE,  COBALTOUS 


Cobaltous  dimetaphosphate,  Co2(P2O6)2. 

Insol.  in  cold  cone.  H2SO4;  si.  sol.  on 
warming,  but  sol.  in  H2O  after  treating  with 
H2SO4.  Sol.  in  cone.  NH4OH+Aq.  Scarcely 
attacked  by  boiling  Na2S+Aq.  (Fleitmann.) 

Cobaltous  hexametaphosphate  (?). 

Ppt.  Sol.  in  sodium  hexametaphosphate  + 
Aq.  (Rose,  Pogg.  76.  4.) 

Cobaltous    orthophosphate  i     Co3(PO4)2  + 

zH2O. 
Sol.  in  H3PO4+Aq  or  NH4OH+Aq;  si.  sol. 

in  NH4C1  or  NH4NO3+Aq.    (Salvetat,  C.  R. 

48.  295.)    Sol.  in  Co  salts  +Aq. 

+2H2O.    (Debray,  A.  ch.  (3)  61.  438.) 
+8H2O.    (Reynoso,  C.  R.  34.  795.) 

Cobaltous  hydrogen  orthophosphate. 


Ppt.    (Debray.) 

+2^H2O.     Ppt.     Insol.  in  H2O.     Sol.  in 
H3PO4+Aq.    (Bodeker,  A.  94.  357.) 

Cobaltous  telrahydrogen.  orthophosphate, 

CoH4(P04)2 
Sol.  in  H2O.    (Reynoso.) 

Cobaltous  pyrophosphate. 
.    Ppt.    Sol.  in  Na4P2O7+Aq.     (Stromeyer.) 
Sol.  in  NH4OH+Aq.     (Schwarzenberg.) 

Cobaltous  pyrometaphosphate,  3CoO,  2P2O5. 
(Braun.) 
6CoO,  5P2O5.    (Braun.) 

Cobaltous  potassium  phosphate,  CoKPO4. 

Insol.   in   H2O;   easily  sol.   in   dil.   acids. 
(Ouvrard,  C.  R.  106.  1729.) 

3CoO,  3K2O,  2P2O5.    As  above. 

Cobaltous  sodium  ^'phosphate,  NaCo2P3Oi0. 
(Schwarz,  Z.  anorg.  1895,  9.  260.) 
Na3CoP3Oio+12H2O.     Very  sol.  in  H2O; 

decomp.    in    aq.    solution.      Sol.    in    acids. 

(Schwarz,  Z.  anorg.  1895,  9.  258.)     . 

Cobaltous  sodium  raetaphosphate. 

Co3Na2(P03)8. 

Insol.  in  H2O  or  acids,  even  cone.  H2SO4. 
(Watts'  Diet.) 

Cobaltous  sodium  worwwietaphosphate, 

6Co(PO3)2,  2NaPO3. 

Insol.  in  H2O  and  dil.  acids.    Sol.  in  cone. 
H2SO4.    (Maddrell,  A.  61.  57.) 

Cobaltous  sodium  Jnraetophosphate. 

CoNa.1(PO3)3+8H2O. 
Sol.  in  H2O.     (Fleitmann  and  Henneberg, 
A.  65.  315.) 


Cobaltous  sodium  orthophosphate,  CoNaPO4. 
Insol.  in  H2O.  (Ouvrard,  C.  R.  106.  1729.) 
Co3(PO4)2,  2Na2HPO4+8H2O.  (Debray, 

J.  Pharm.  (3)  46.  119.) 

Cobaltous  sodium  pyrophosphate, 

Co10Nai6(P2O7)9. 

Insol.  in  H2O.    Sol.  in  acids.     (Wallroth.) 
+zHoO.    Sol.  in  H2O.    (Stromeyer.) 

Cobaltous  zinc  phosphate,  Co3(PO4)2, 

3Zn3(PO4)2  +  12H2O. 
Ppt.    Sol.  in  acids.    (Gentele.) 
CoZn2(PO4)2+6H2O.    Insol.  in  H2O. 

Columbium  phosphate  (?) 

Insol.  in  H2O.     (Blomstrand.) 

Cupric  diraetaphosphate,   Cu2(P2O6)2. 

Insol.  in  H2O.  Sol.  in  cone.  H2SO4.  (Mad- 
drell, A.  61.  62.)  Insol.  in  most  cone,  acids 
and  in  alkalies,  except  hot  NH4OH+Aq  or 
cone.  H9SO4,  in  which  it  is  moderately  sol. 

Not  decomp.  by  H2S,  but  by  (NH4)2S+Aq, 
less  easily  by  Na2S,  and  K2S-j-Aq.  (Fleit- 
mann, Pogg.  78.  242.) 

+8H2O.  Completely  insol.  in  H2O.  (Fleit- 
mann.) 

Cupric  /lezametophosphate  (?). 

Sol.  in  Na8P6O18+Aq  or  CuCl2+Aq. 
(Rose,  Pogg.  76.  5.) 

Cu3P6Ol8.  Easily  sol.  in  H2O  or  acids, 
especially  when  freshly  pptd.  (Liidert,  Z. 
anorg.  5.  15.) 

Cupric  orthophosphate.  basic,  6CuO.  P2O5  + 
3H20. 

Min.  Phosphocalcite. 

5CuO,  P2O5+2H2O.    Min.  Dihydrite. 

+3H2O.  Min.  Ehlite.  Easily  sol.  in 
NH4OH+Aq,  and  HNO3+Aq. 

4  CuO,  P2O5+H2O.  Slowly  sol.  in  NH4OH 
or  (NH4)2CO3+Aq;  insol.  in"  cold  Na2S2O3  + 
Aq.  (Steinschneider,  C.  C.  1891,  II.  51.) 

SI.  sol.  in  CuCl2+Aq  and  CaSp4+Aq 
Decomp.  by  boiling  H2O  and  boiling  Aq 
potash.  (Caven,  J.  Soc,  Chem.  Ind.  1897, 
16.  29.) 

Min.  Inbethenite.  Sol.  in  acids  and 
NH4OH+Aq. 

+2H.O.  Min.  Pseudolibethenite.  Sol.  in 
acids  and  NH4OH+Aq. 

+3H2O.  Min.  Tagilite.  Sol.  in  acids  and 
NH4OH+Aq. 

Cupric  ^nphosphate,  5CuO,  3P2O5  +  13H2O. 

Sol.  in  H2O.  Sol.  in  HNO3.  (Schwarz,  Z. 
anorg.  1895,  9.  262.) 

Cupric  dimetaphosphate t  CuP2O6+4H2O. 

Sol.  in  78  pts.  H2O.  Easily  decomp.  by 
hot  cone.  H2SO4.  (Glatzel,  Dissert.  1880.) 


PHOSPHATE,  CUPRIC  URANYL 


691 


Cupric  /n'wetaphosphate,  C 

Very  si.  sol.  in  H2O  (0.04  g.  in  1  1.  at  20°) 
(Tammann,  J.  pr.  1S92,  (2)  45.  425.) 

Cupric  tetrametaphosphsite,  Cii2P4Oi2. 

Insol.  in  H2O  and  in  HC1.  SI.  sol.  in  boiling 
HNO3.  Very  sol.  in  boiling  cone.  H2SO4 
(Glatzel.) 

-f8H2O.  Nearly  insol.  in  H2O.  Slowly 
attacked  by  acids  except  cone.  H2SO4 
(Glatzel.) 

Cupric    ortfiophosphate,      Cu3(PO4)2+3H2O. 

Insol.  in  H2O;  easily  sol.  in  acids,  even 
H3PO4,  HC2H3O2,  or  H2SO3+Aq.  Sol.  in 
NH4OH+Aq.  SI.  sol.  in  NH4  salts  +Aq. 

SI.  sol.  in  Cu  salts  +Aq.  (Rose,  Pogg.  76. 
25.) 

Sol.  in  cold  Na2S2O3+Aq.  (Steinschnei- 
der,  C.  C.  1891,  II,  51.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  827.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Cupric    hydrogen    phosphate,    CuHPO4  + 


Insol.  in  H2O;  sol.  in  H3PO4+Aq,  and 
HC2H3O2+Aq.  Insol.  in  NH4C1,  and 
NH4NO3+Aq.  (Brett,  Phil.  Mag.  (3)  10. 
98.) 

Cupric      p?/rophosphate,      basic.      Cu2P2O7, 

2CuO,  H2O+3H2O. 
Insol.  in  H2O.    (Pahl,  J.  B.  1873.  229.) 

Cupric  pj/rophosphate,  Cu2P2O7. 

Anhydrous.  Insol.  in  H2O,  and  very  si. 
sol.  in  cone,  acids.  (Fleitmann,  Pogg  78. 
244.) 

As  insol.  as  Cu  metaphosphate,  but  de- 
comp.  by  H2S.  (Rose,  Pogg.  76.  14.) 

+2H2O.  Sol.  in  mineral  acids,  and  NH4OH 
+Aq;  also  in  Na4F2O7+Aq.  (Sehwarzen- 
berg,  A.  66.  156.) 

Sol.  in  cold  H2SO3-j-Aq  without  decomp., 
crystallizing  out  on  boiling. 

Decomp.  by  boiling  KOH+Aq. 

Sol.  in  large  excess  of  CuSO4+Aq. 

+2^H2O.    (Pahl,  Sv.  V.  A.  F.  30,  7.  40.) 

-f5H2O.    Very  si.  sol.  in  H2O. 

Sol.  in  dil.  acids.  (Wiesler,  Z.  anorg.  1901, 
28.  202.) 

Cupric   iron    (ferric)    pz/rophosphate, 

Cu3Fe2(P2O7)3  +  12H2O. 
Ppt.    (Pascal,  C.  R.  1908,  146.  2.33.) 

Cupric    potassium    phosphate,    4CuO,    K2O, 
3P2O.5. 

Insol.  in  H2O.    COuvrard,  C.  R.  111.  177.) 
CuKPO4.    As  above. 


Cupric  potassium  teft*ametaphosphate, 

K2CuP4O12+4H2O. 

Sol.  in  58  pts.  H2O.  Easily  attacked  by 
acids'.  (Glatzel,  Dissert.  1880.) 

Cupric  potassium  pyrophosphate,  CuK2P2O7. 

Extremely  easily  sol.  in  H2O.  (Persoz,  A. 
ch.  (3)  20.  315.) 

Cu2P2O7,  3K4P2O7+4H2O.  Insol.  in  H2O. 
(Pahl,  Sv.  V.  A.  F.  30,  7.  44.) 

Cupric  sodium  phosphate,  Cu3Na6(PO4)4. 

Insol.  in  HC2H3O2+Aq.  Sol.  in  cone. 
acids.  (Wallroth,  Bull.  Soc.  (2)  39.  316.) 

Cupric  sodium  inphosphate, 
CuXa3P3Oio+12H2O. 

SI.  sol.  in  H2O;  very  unstable. 

Easily  sol.  in  acids.  (Stange,  Z.  anorg. 
1896,  12.  458.) 

Cupric   sodium  tetrametaphosphate, 
CuNa2P4Oi2. 

As  insol.  in  H2O  as  Cu  dimetaphosphate. 
Difficultly  decomp.  by  digestion  with  Na2S-f 
Aq.  (Fleitmann,  Pogg.  78.  355.) 

+4H2O.  Sol.  in  45  pts.  H2O.  (Glatzel, 
Dissert.  1880.) 

Cupric  sodium  or^Aophosphate,  3Cu3(PO4)2, 
NaH2PO4. 

Decomp.  by  H2O  to  4CuO,  P2O5.  (Stein- 
schneider,  C.  C.  1891,  II.  52.) 

2Cu3(PO4)2,  Na2HPO4.  Decomp.  by  H2O 
into  —  • 

3Cu3(PO4)2,  Na2HPO4.  Decomp.  by  H2O. 
(S.) 

Cu3(PO4)2,  NaH2PO4.  Decomp.  by  H2O. 
(S.) 

6Cu3(PO4)2,  2Na3PO4.     Decomp.  by  H2O. 


Cupric  sodium  p^/rophosphate,    CuNa2P2O7. 

Insol.  in  H2O.  (Fleitmann  and  Henne- 
berg,  A.  65.  387.) 

+2/3H2O.  (F.  and  H.)  Much  more  sol. 
than  the  next  salt.  (Pahl.) 

+6H2O.    (Persoz,  A.  ch.  (3)  20.  315.) 

Cu2P2O7,  CuNaaP2O7+3^H2O.  Very  ef- 
florescent; insol.  in  H2O.  (F.  and  H.) 

+  10^H2O.    (Pahl,  Sv.  V.  A.  F.  30,  7.  42. 

CuNa2P2O7,  Na4P2O7.  Sol.  in  H2O.  (-F. 
and  H.) 

+2H2O.    (F.  amd  H.) 

+  12,  and  16H2O.  Very  efflorescent,  and 
sol.  in  H2O.  (Pahl.) 

Cu3Na2P4Oi4+10H2O.  Insol.  in  H2O; 
sol.  in  HC1  and  HNO3  even  after  heating. 
(Stange,  Z.  anorg.  1896,  12.  456.) 

Cupric  uranyl  phosphate,  (UO2)2Cu(PO4)2  + 
8H2O. 

Insol.  in  H2O;  easily  sol.  in  acids.  (De- 
Dray.) 

Min.  Chalcolite.    Sol.  in  HNO3+Aq. 


692 


PHOSPHATE,  CUPRIC,  AMMONIA 


Cupric  orthophosphate  ammonia,  Cu3(PO4)2, 
4NH3. 

SI.  sol.  in  H2O.  Easily  sol.  in  H2O  contain- 
ing NH4OH.  (Schiff,  A.  123.  41.) 

2CuO,  3P2O5,  20NH3+21H2O.  Easily 
sol.  in  cold  H2O,  with  subsequent  decomp. 
(Metzner,  A.  149.  66.) 

2CuO,  P2O5,  6NH3.     (Maumene\) 

Cupric    p«/rophosphate    ammonia,    SCuO, 
3P2O5,  4NH3+4H2O. 

SI.  sol.  in  H2O.  (Schwarzenberg,  A.  66. 
133.) 

Cu2P2O7,  4NH3+H2O.  SI.  sol.  in  H2O. 
(Schiff,  A.  123.  1.) 

Didymium  raetaphosphate,  Di(PO3)3. 
Precipitate.    (Smith.) 
Di2O3,  5P2O5.     Insol.  in  H2O.     (Cleve.) 

Didymium  phosphate,  2Di2O3,  3P2O5. 
Insol.  in  H2O.    (Ouvrard,  C.  R.  107.  37.) 

Didymium  or^ophosphate,  DiPO4. 

Insol.  in  H2O.  Very  si.  sol.  in  dil.,  easily 
sol.  in  cone,  acids.  (Marignac.)  Insol.  in 
H2O.  (Wallroth,  Bull.  Soc.  (2)  39.  316.) 

+H2O.  (Frerichs  and  Smith,  A.  191. 
355.) 

Didymium  ^nhydrogen  phosphate, 

Di2H3(P04)3. 

Precipitate.     (Frerichs  and  Smith.) 
Existence  is  doubtful.    (Cleve,B.    12.  910.) 

Didymium    hexahydrogen    phosphate, 

DiH3(PO4)2+H2O. 
Precipitate.     (Hermann.) 

Didymium    pyrophosphate,     Di4(P2O7)3-f 

6H2O. 
Precipitate.    (Cleve.) 

Didymium  hydrogen  pz/rophosphate, 
Di2H6(P2O7)3. 

Precipitate.  Sol.  in  disodium  pyrophos- 
phate+Aq.  (Frerichs  and  Smith,  A.  191. 
355.) 

Does  not  exist.    (Cleve.) 

Didymium    potassium    phosphate,    2Di2O3, 

3K2O,  3P2O6  =  2DiPO4,  K3PO4. 
Insol.  in  H2O.    (Ouvrard,  C.  R.  107.  37.) 

Didymium    sodium   ortAophosphate,    Di2O3, 

3Na2O,  2P2O8  =  DiPO4,  Na3PO4. 
Insol.  in  H2O.    (Ouvrard.) 

Didymium  sodium  p?/rophosphate,  Di2O3, 

Na2O,  2P2O5  =  DiNaP2O7. 
Insol.  in  H2O.    (Ouvrard,  C.  R.  107.  37.) 


Dysprosium  orf/iophosphate,  DyPO4+5H2O. 

Nearly  insol.  in  H2O. 

Easily  sol.  in  dil.  acids  or  acetic  acid. 
(Jantsch,  B.  1911,  44.  1276.) 

Erbium  phosphate,  ErPO4+H2O. 

Precipitate. 

Erbium  p?/rophosphate,  ErHP2O7+3KH2O. 
Scarcely  sol.  in  boiling  H2O.     Slowly  sol. 
in  acids. 

Erbium  sodium  p?/r0phosphate,  ErNaP2O7. 
Precipitate.    ^Wallroth.) 

Glucinum  metophosphate,  G1(PO3)2. 

Insol.  in  H2O  ana  acids.  (Bleyer,  Z.  anorg. 
1912,  79.  274. 

Glucinum  or^ophosphate,  basic. 

2G13P2O8,  G1O  +  13H2O. 
Ppt.     (Bleyer,  Z.  anorg.  1912,  79.  268.) 

Glucinum  ort/iophosphate,  G13(PO4)2+6H2O. 

Precipitate.  Insol.  in  H2O.  Sol.  in  acids. 
(Atterberg,  Sv.  V.  A.  Handl.  12,  6.  33.) 

1  1.  2%  HC2H3O2+Aq  dissolves  0.55  g.  of 
the  anhydrous  salt;  1  1.  10%  HC2H3O2+Aq 
dissolves  1.725  g.  (Sestini,  Gazz.  ch.  it.  20. 
313.) 

+7H2O.    (Atterberg.) 

Glucinum  hydrogen  or^ophosphate,  G1HPO4 
+3H20. 

G1H4(PO4)2    hydroscopic.      (Bleyer,    Z. 
anorg.  1912,  79.  266.) 

Precipitated  by  alcohol.     (Atterberg.) 

Glucinum  phosphate,  5G1O,  2P2O5+8H2O. 
Ppt.    Sol.  in  H2O  with  decomp.    (Scheffer.) 
3G1O,  P2O5,  3H2O+H2O.     (Sestini,  Ga/z. 

ch.  it.  20.  313.) 

Glucinum  p?/rophosphate,  G12P207+5H2O. 

Precipitate.     (Scheffer.) 

Sol.  in  Na4P2O7+Aq.      (Stromeyer.) 

Glucinum  potassium  phosphate,  G1KPO4. 
Insol.  in  H2O.    (Ouvrard,  C.  R.  110.  1333.) 

Glucinum    sodium   phosphate,    GlNaPO4. 

SI.  sol.  in  cold,  easily  sol.  in  hot  acids. 
(Wallroth.)    Insol.  in  acetic  acid. 

Min.      Beryllonite. 

G1O,  2Na2O,  P2O5.  Insol.  in  H2O.  (Ouv- 
rard, C.  R.  110.  1333.) 

Gold   (Auric)   sodium  pT/rophosphate   (?), 

Au4(P2O7)3,  2Na4P2O74-H2O. 
Sol.inH2O.    (Persoz.) 


PHOSPHATE,  IRON 


693 


Gold   sodium    pyrophosphate,   ammonia, 

14Au2Os,  6P2OS,  3Na2O,  14NH3+24H2O. 
Insol.  in  H2O.     (Gibbs,  Am.  Ch.  J.  1895, 
17.  172.) 

Iron  (ferrous)  inmetophosphate,  Fe(P3O9)3  + 

12H2O. 

Rather  si.  sr>l.  in  cold,  more  easily  in  hot 
H2O.  After  ignition  sol.  in  HCl+Aq  only 
after  long  boiling.  (Liridbom,  Acta  Lund. 
1873.  17.) 

Ferrous  hexametaphosphate,  Fe3P6Oi8. 

When  freshly  pptd.  is  sol.  in  H2O,  and  very 
sol.  in  least  traces  of  acids,  or  Na6P6Oi8+Aq. 
(Liidert,  Z.  anorg.  5.  15.) 

Ferrous    phosphate,    basic,    7FeO,    2P2O5  + 

9H2O. 

Min.  Ludlamite.  Sol.  in  dil.  H2SO4  or 
HCl+Aq.  Decomp.  by  boiling  KOH  or 
NaOH+Aq. 

Ferrous  orZAophosphate,  Fe3(PO4)2. 

Insol.  in  H2O;  sol.  in  acids. 

Sol.  in  1000  pts.  H2O  containing  more  than 
1  vol.  CO2.  (Pierre.) 

Sol.  in  an  excess  of  ferrous  salts  +Aq. 

Sol.  in  560  pts.  H2O  containing  V56o  pt. 
HC2H3O2.  Sol.  in  1666  pts.  H2O  containing 
150  pts.  NH4CoH3O2.  (Pierre,  A.  ch.  (3)  36. 
78.) 

Sol.  in  NH4  salts +Aq. 

Sol.  in  NH4OH+Aq.  Not  pptd.  in  pres- 
ence of  Na  citrate. 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

+H2O.    (Debray,  A.  ch.  (3)  61.  437.) 

+8H2O.  Min.  Vivianite.  Easily  sol.  in 
HC1  or  HNOs+Aq.  Boiling  KOH+Aq  dis- 
solves out  phosphoric  acid.  Sol.  in  cold  citric 
acid+Aq.  (Bolton,  C.  N.  37.  14.) 

Insol.  in  H2O.  Sol.  in  acids.  (Evans,  C.  C. 
1897,  I.  580.) 

Ferrous  hydrogen  or^ophosphate,  FeHPO4+ 

H2O. 

Ppt.    (Debray,  A.  ch.  (3)  61.  437.) 
Is   impure   Fe3(PO4)2.      (Erlenmeyer   and 

Heinrichs,  A.  194.  176.) 

Ferrous  tetrahydrogen  or^Aophosphate, 

FeH4(P04)2+H20. 

Easily  sol.  in  H2O.  Not  changed  by  al- 
cohol. (Erlenmever  and  Heinrichs,  A.  194. 

176.) 

Ferrous  p^/rophosphate. 

Ppt.  Sol.  in  an  excess  of  Na4P2O7  or  FeSO4 
+Aq.  (Schwarzenberg,  A.  65.  153.) 

Ferric  7wetophosphate,  Fe3(PO3)6  or  Fe(PO3)3. 
Insol.  in  H2O  or  dil.  acids.     Sol.  in  cone. 
H2SO4.    (Maddrell,  Phil.  Mag.  (3)  30.  322.) 


Iron  (ferric)  orthophosphate,  basic,  2Fe2O3, 
P2O5+zH2O. 

Insol.  in  NH4  citrate,  sol.  in  NH4  tartrate 
+Aq.  (Wittstein.) 

+3H-X).  Min.  Krauri'.e.  Easily  sol.  in 
HCl+A~q. 

+4H2O.    Ppt.    (Millot,  C.  R.  82.  89.) 

+5H2O.    Min.  Dufrenite. 

+  12H2O.  Min.  Cacoxene.  Sol.  in  HC1  + 
Aq. 

+  18,  or  24H2O.    Min.  Delvauxite. 

5Fe2O3,  3P,Od  +  14H2O.  Min.  Beraunile. 
Sol.  in  HCl+Aq. 

3Fe2O3,  2P2O5+8H2O.  Min.  Eleonorite. 
Sol.  in  HCl+Aq. 

Ferric  ortfiophosphate,  Fe2(PO4)2+:rH2O,  or 
2Fe2O3,  3P205+zH2O. 

+4,  or  8H2O.  (Pptd.  ferric  phosphate.) 
Insol.  in  H2O.  Sol.  in  1500  pts.  boiling  H2O. 
(Bergmann,  1815.)  Sol.  in  pure  H2O  when 
all  traces  of  soluble  salts  are  absent.  (Frese- 
nius.)  Very  si.  sol.  in,  but  decomp.  by  H2O. 
(LachowiczJ  W.  A.  B.  101,  2b.  374.)  For  an 
extended  discussion  of  solubility  in  and  de- 
composition by  H2O  and  effect  of  salts  see 
Cameron  and  Hurst,  (J.  Am.  Chem.  Soc.  1904, 
26.  888.) 

Easily  sol.  in  dil.  mineral  acids,  excepting 
H3PO4+Aq.  Insol.  in  cold  HC2H3O2+Aq. 
(Wittstein.)  100  ccm.  cold  H2O  containing 
10%  HC2H3O2  dissolve  0.007  g.  salt.  (Ses- 
tini,  Gazz.  ch.  it.  5.  252.)  When  freshly  pptd. 
easily  sol.  in  H2SO3+Aq,  or  (NH4)2SO3+Aq. 
(Berthier.)  Easily  sol.  in  tartaric  or  citric 
acid+Aq,  also  in  NH4  salts  of  those  acids, 
and  Na  citrate+Aq.  (Heydenreich,  C.  N.  4. 
158.)  See  below. 

Sol.  in  12,500  pts.  H2O  sat.  with  CO2. 
(Pierre,  A.  ch.  (3)  36.  78.) 

Insol.  in  NH4  salts +Aq.  (Wittstein.) 
Sol.  in  NH4OH+Aq  in  presence  of  Na2HPO4; 
insol.  in  hot  Na2HPO4+Aq;  sol.  in  (NH4)2CO8 
+Aq  (Berzelius).  NH4OH,  KOH,  or 
NaOH+Aq  dissolve  out  H3PO4. 

Sol.  in  ferric  salts +Aq,  even  ferric  acetate, 
but  insol.  in  ferrous  acetate+Aq. 

Partially  sol.  in  large  amt.  of  Na2CO3+Aq. 
Not  pptd.  in  presence  of  Na  citrate.  (Spiller.) 

Arth  (Bull.  Soc.  (3)  2.  324)  obtained  a 
modification  of  Fe2(PO4)2,  insol.  in  HNO3  + 
Aq,  but  sol.  in  hot  cone.  HCl+Aq. 

+4H2O.  Min.  Strengite.  Easily  sol.  in 
HCl+Aq;  insol.  in  HNO3+Aq. 

+5H2O.  Only  si.  sol.  in  H2O.  Slowly  sol. 
in  HNO3,  easily  sol.  in  HC1.  (Weinland,  Z 
anorg.  1913,  84.  361.) 

Diammonium  citrate  +Aq  dissolves  4.8% 
of  the  P2O5;  triammonium  citrate,  5.8%  P2O6; 
and  with  an  excess  of  NH4OH,  21.2%  P2O6 
is  dissolved.  (Erlenmej^er,  B.  14.  1253.) 

+9H2O.  Dissolves  in  35  min.  in  diam- 
mpnium  citrate  +Aq  (sp.  gr.  1.09);  in  55 


mm.  in  triammonium  citrate   +Aq  (sp.  gr. 
Q  (1A%  citric  acid)  dis- 
solves 17.5%  of  the  P2O5.    (Erlenmeyer,  I.  c.} 


1.09);  citric  acid  +Aq  (l/i%  citric  acic 


694 


PHOSPHATE,  IRON,  ACID 


Iron  (ferric)  phosphate,  acid,  8Fe2O3,  9P2O5 
+3H2O. 

Insol.  in  H2O.    (Riimpler,  Z.  anal.  12.  151.) 

6Fe2O3,  7P2O5+3H2O. 

4Fe2O3,  5P2O5+3H2O. 

2Fe2O3,  3P2O5+8H2O.  Ppt.  Decomp.  by 
H2O  finally  into  Fe2(PO4)2.  (Erlenmeyer  and 
Heinrich,  A.  194.  176.) 

8Fe2O3,  11P2O5+9H2O.  As  above.  (E. 
and  H.) 

4Fe2O3,  7P2O5+9H2O.  As  above.  (E.  and 
H.) 

Fe2O3,  2P2O5+8H2O.  Insol.  in  H2O  or 
HC2H3O2+Aq;  sol.  in  NH4  citrate,  alkali 
hydrates,  or  carbonates  +Aq.  (Winkler.) 
Slowly  decomp.  by  H2O.  (E.  and  H.) 

+  10H2O.    (Waine,  C.  N.  36.  132.) 

2Fe2O3,  5P2O5  +  17H2O. 

Fe2O3,  3P2O5+6H2O  =  FeH€(PO4)3.  Deli- 
quescent. Insol.  in  H2O,  but  decomp.  into 
Fe2(PO4)2.  (E.  andH.) 

+4H2O.  (Hautefeuille  and  Margottet, 
C.  R.  106.  135.) 

Ferric  pz/rophosphate,  Fe4(P2O7)3. 

Two  modifications. — (a)  Sol.  in  acids, 
Na4P2O7+Aq,  FeCl3+Aq,  NH4OH+Aq,  and 
in  (NH4)2CO3+Aq. 

Insol.  in  acetic,  sulphurous  acid,  or  NH4C1 
+Aq.  Sol.  in  NH4  citrate+Aq.  (Schwarzen- 
berg,  A.  65.  153.) 

(6)  Insol.  in  dil.  acids,  Na4P2O7+Aq,  FeCl3 
+Aq.  Sol.  in  IsH4OH+Aq.  (Gladstone, 
Chem.  Soc.  (2)  6.  435.) 

Solubility  of  Fe4(P2O7)3  in  NH4OH+Aq  at  0°. 


100  g.  sat.  solution  contain 

100  g.  sat.  solution  contain 

G.  NH3 

G.  Fe4(P207)3 

G.  NHs 

G.Fe4(P2O7)3 

0.884 
1.59 
3.71 
4.72 
5.93 
7.91 

5.606 
9.75 
14.85 
15.94 
13.92 
14.61 

5.92 
8.26 
10.55 
15.96 

18.83 

14.71 
13.89 
7.40 
2.52 
0.445 

(Pascal,  A.  ch.  1909,  (8)  16.  374.) 

Insol.  in  acetone.  (Krug  and  M'Elroy,  J. 
Anal.  Appl.  Ch.  6.  184.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.). 

Ferroferric       or^/iophosphate,       2Fe3(PO4)2, 

3(Fe*O3,  2P2O5)  +  16H2O. 
Ppt.    Sol.  in  HCl+Aq.    (Rammelsberg.) 
4Fe2O3,  6FeO,  5P2O5+40H2O.     Sol.  in' 40 
min.  in  diammonium  citrate+Aq  (sp.  gr.  = 
1.09);   triammonium   citrate+Aq   (sp.   gr.  = 
1.09)  dissolves  55.7%  of  the  P2O6.     (Erlen- 
meyer, B.  14.  1253.) 

Ferrous  lithium  phosphate,  Li3PO4,  Fe3(PO4)2. 
Min.  Triphylline.    Easily  sol.  in  acids;  not 
wholly  decomp.  by  KOH+Aq. 


Iron  (ferrous)  manganous  phosphate, 

Fe3(PO4)2,  Mn3(PO4)2. 
Min.  Triplite.    Easily  sol.  in  HCl+Aq. 
5(Mn,Fe)O,    2P2O5+5H2O.      Min.    Hur- 
eaulite.    Sol.  in  acids. 

Ferric   manganous    sodium    phosphate, 

FePO4,  (Na2,Mn)3PO4+}^H2O. 
Min.—  (?). 

Ferrous     manganous     phosphate     chloride, 

3(Mn,Fe)3(PO4)2,  MnCl2. 
(Deville  and  Caron.) 

Ferrous  manganous  phosphate  fluoride, 

(Mn,Fe)s(PO4)2,  (Mn,Fe)F2. 
Min.  Triplite,  Zwielesite.    Sol.  in  HCl+Aq. 
3(Mn,Fe)3(PO4)2,    MnF2.      (Deville    and 
Caron,  C.  R,  47.  985.) 

Ferric  potassium  phosphate,  2Fe2O3,  3K2O, 
3P205. 

Not  attacked  by  boiling  H2O.  (Ouvrard, 
A.  ch.  (6)  16.  289.) 

Fe2O3,  K2O,  2P2O5.  Insol.  in  H2O;  very  si. 
attacked  by  acids.  (Ouvrard.) 

Ferric  silver  wetophosphate,  2Fe2O3,  2Ag20, 

5P2O5. 

(Hautefeuille  and  Margottet,  C.  R.  96. 
1142.) 

Ferric  silver  p?/rophosphate,  Fe2Ag6(P2O7)3  + 

4H2O. 
Ppt.    (Pascal,  C.  R.  1908,  146.  232.) 

Ferric    sodium   phosphate,    2P"e2O3,    3Na2O, 

3P205. 
Decomp.  by  H2O.    (Ouvrard.) 

Ferrous  sodium  /n'phosphate,   FeNa3P3Oio+ 


Stable  dry;  sol.  in  HNO3:  decomp.  in  con- 
tact with  H,O.  (Stange,  Z.  anorg.  1896,  12. 
451.) 


Ferric     sodium     hydrogen 
Fe(PO4)2H2Na+H2O. 


or^ophosphate, 


Difficultly  sol.  in  H2O.  Slowly  decomp.  by 
boiling  with  H2O.  Sol.  in  dil.  HC1  and  dil. 
HNO3.  Decomp.  by  alkalies  and  alkali  car- 
bonates. (Weinland,  Z.  anorg.  1913,  84.  354.) 

Fe(PO4)3H5Na+H2O.  Difficultly  sol.  in 
H2O.  Decomp.  by  boiling  with  H2O.  Sol.  in 
dil.  HC1  and  in  dih  HNO3.  Decomp.  by  al- 
kalies and  alkali  carbonates.  (Weinland,  Z. 
anorg.  1913,  84.  358.) 

Ferric  sodium  p?/rophosphate,  Fe4(P2O7)3, 
2Na4P207+7H20 

Slowly  but  completely  sol.  in  H2O.  Pptd. 
by  alcohol.  (Milck,  J.  B.  1865.  263.) 

Very  sol.  in  H2O.  (Fleitmann  and  Henne- 
berg.) 


PHOSPHATE,  LEAD  SODIUM 


695 


+5,  and  6H2O.  Easily  sol.  in  H2O,  espe- 
cially if  warm.  (Pahl,  J.  B.  1873.  229.) 

FeNaP2O7.  Insol.  in  H2O,  dil.  HC1,  or 
HNOa+Aq;  si.  sol.  in  cone.  HCl+Aq;  de- 
comp. by  cone,  hot  H2SO4  without  solution. 
(Jorgensen,  J.  pr.  (2)  16.  342.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Na6Fe2(P2O7)3+9H2O.  Decomp.  by  H2O. 
(Rosenheim,  B.  1915,  48.  586.) 

Fe4(P2O7)3,  5Na4P2O7+7H2O.  (Pahl,  J.  B. 
1873.  229.) 

Iron  (ferric)  phosphate  sulphate,  3Fe2(PO4)2, 

2Fe2(SO4)3,  2Fe2O6H6. 
Min.  Diaochite. 

Lanthanum  raetaphosphate,  La2(PO3)6. 
Precipitate.    (Frerichs  and  Smith.) 
La2O3,  5P2O5.    Insol.  in  H2O,  dil.,  or  cone. 

acids.    (Johnsson,  B.  22.  976.) 

Lanthanum  or£/iophosphate,  LaPO4. 

Precipitate.    (Hermann.) 

Insol.  in  H2O  and  acids.  (Ouvrard,  C.  R. 
107.  37.) 

Lanthanum  hydrogen  phosphate, 

La2H3(P04)3. 

Precipitate.    (Frerichs,  B.  7.  799.) 
Existence  is  doubtful.    (Cleve,  B.  11.  910.) 

Lanthanum  phosphate,  acid,  La2O3,  2P2O5. 
Precipitate.    (Hermann.) 

Lanthanum  p?/rophosphate,  LaHP2O7+3H2O. 

(Cleve.) 

La2H6(P2O7)3.  Precipitate.  (Frerichs  and 
Smith.) 

Does  not  exist.    (Cleve.) 

Lanthanum  potassium  or//iophosphate, 

2La2O3,  3K2O,  3P2O5  =  2LaPO4,  K3PO4. 
Insol.  in  H2O.    (Ouvrard,  C.  R.  107.  37.) 

Lanthanum  sodium  ort/iophosphate,  La2O3, 

3Na2O,  2P2O5. 
Insol.  in  H^O.    (Ouvrard.) 

Lanthanum  sodium  p?/rophosphate, 

LaNaP2O7. 

Insol.  in  acetic,  and  dil.  cold  mineral  acids. 
Sol.  in  warm  dil.  acids.  fWallroth.) 


Lead  dirae/aphosphate, 

Ppt.  Almost  insol.  in  H2O.  Sol.  in  HNO3 
+Aq.  (Fleitmann,  Pogg.  78.  253.) 

Lead  inwetophosphate,  Pb3(P3O9)2+3H2O. 

Nearly  insol.  in  H2O.  Less  sol.  in  H2O 
than  the  corresponding  Ag  salt.  (Fleitmann 
and  Henneberg,  A.  66.  304.) 

Most  insol.  of  the  tfnmetaphosphates. 
(Lindbom,  Acta  Lund.  1873.  12.) 


Anhydrous  salt  is  insol.  in  H2O;  easily  sol. 
in  HNO3+Aq.    (Lindbom.) 


Lead  fe^rametophosphate, 

Insol.  in  H2O. 

More  easily  decomp.  by  acids  than  the  other 
insol.  metaphosphates.  Easily  decomp.  by 
alkali  hydrosulphides+Aq  in  the  cold. 
(Fleitmann,  Pogg.  78.  353.) 

Lead  hexametaphosphate,  PbsPeOis. 

Nearly  insol.  in  H2O;  sol.  in  acids.  (Lii- 
dert,  Z.  anorg.  5.  15.) 

Lead  or/ftophosphate,  basic,  4PbO,  P2O5. 
(Gerhardt,  A.  72.  85.) 

Lead  or/Aophosphate,  Pb3(PO4)2. 

Insol.  in  H2O;  sol.  in  HNO3+Aq.  Insol. 
in  HC2H3O2+Aq. 

SI.  sol.  in  H2O.  1.35  X10-4  g.  is  contained 
in  1  litre  of  sat.  solution  at  20°.  (Bottger,  Z. 
phys.  Ch.  1903,  46.  604.) 

Not  hvdrolyzed  by  boiling  H2O.  Sol.  in 
boiling  KOH+Aq;  insol.  in  NH4OH+Aq. 
Insol.  in  Pb(NO3)2+Aq.  (Caven,  J.  Soc. 
Chem.  Ind.  1897,  16.  30.) 

Sol.  in  782.9  pts.  HC2H3O2+Aq  containing 
38.94  pts.  pure  HC2H3O2.  (Bertrand,  Monit. 
Scient.  (3)  10.  477.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

Lead  hydrogen  phosphate,  PbHPO4. 

Insol.  in  H2O.  Decomp.  by  H2SO4,  or  HC1 
+Aq.  Sol.  in  HNO5,  or  in  KOH  or  NaOH+ 
Aq.  Insol.  in  HC2H3O2+Aq.  Sol.  in  cold 
NH4Cl+Aq  (Brett),  from  which  it  can  be 
completely  precipitated  by  a  great  excess  of 
NH4OH+Aq. 

More  sol.  in  NH4C2H3O2+Aq  at  18.8-25° 
than  in  pure  H2O.  (Wappen.) 

Sol.  in  sat.  NaCl+Aq,  but  less  than  PbSO4. 
(Becquerel,  C.  R.  20.  1524.) 

Insol.  in  Pb  salts  +Aq. 

Not  pptd.  in  presence  of  Na  citrate 
(Spiller.) 

Lead  pyrophosphate,  Pb2P2O7+H2O. 

Insol.  in  H2O.  Sol.  in  HNO3,  or  KOH+Aq. 
Insol.  in  NH4OH+Aq,  HC2H3O2,  or  SO2  + 
Aq.  (Schwarzenberg,  A.  65.  133.)  Sol.  in 
Na4P2O7+Aq.  (Stromeyer.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Lead  potassium  phosphate,  PbKPO4. 

Decomp.  by  hot  H2O.  (Ouvrard,  C.  R.  110. 
1333.) 

Lead  sodium  phosphate,  PbNaPO4. 

Very  sol.  in  dil.  acids.  (Ouvrard,  C.  R. 
110.  1333.) 

lOPbO,  8Na2O,  9P2O5.    (Ouvrard.) 


696 


PHOSPHATE,  LEAD  SODIUM 


Lead  sodium  pyrophosphate,  PbNa2P2O7. 

Insol.  in  hot  H2O.  (Gerhardt,  A.  ch.  (3) 
22.  506.) 

Lead   Znphosphate     sodium   pyrophosphate, 

Pb5INa4P8O27  +  10H2O. 
Sol.  in  HNO3  after  melting.     (Stange,  Z. 
anorg.  1896,  12.  459.) 

Lead  phosphate  chloride,  2PbHPO4,  PbCl2. 

Insol.  in  boiling  H2O;  sol.  in  dil.  HNO3+ 
Aq.  (Gerhardt,  A.  ch.  (3)  22.  505.) 

2Pb3(PO4)2,  PbCl2.  Ppt.  (Heintz,  Pogg. 
73.  119.) 

3Pb3(PO4)2,  PbCl2.  Min.  Pyromorphite. 
Sol.  in  HNO3,  and  KOH+Aq. 

SI.  sol.  in  cold  citric  acid+Aq.  (Bolton, 
C.  N.  37.  14.) 

+H2O.  Insol.  in  H2O.  Sol.  in  dil.  HNO3 
+Aq.  (Heintz.) 

Lithium  metophosphate,  LiPO3. 

Insol.  in  boiling  H2O.  Scarcely  sol.  in 
acetic  acid.  Easily  sol.  in  mineral  acids. 
(Merling,  Z.  anal.  1879,  18.  565.) 

Lithium  te^raraetaphosphate,  Li4P4Oi2  + 

4H20. 

Very  sol.  in  H2O.  (Warschauer,  Z.  anorg. 
1903,  36.  180.) 

Lithium  or^ophosphate,  Li3PO4. 

Very  slightly  sol.  in  H2O. 

Sol.  in  2539  pts.  pure  H2O  and  3920  pts. 
ammoniacal  H2O;  much  more  readily  in  H2O 
containing  NH4  salts.  Easily  sol.  in  HC1+ 
Aq  or  HNO3+Aq.  (Mayer,  A.  98.  193.) 
Easily  sol.  in  carbonic  acid  water.  (Troost.) 
Sol.  in  dil.  acids  or  acetic  acid,  (de  Schulten, 
Bull.  Soc.  (3)  1.  479.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Insol.  in  acetone.    (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 
rH2O. 


Lithium  hydrogen  phosphate,  Li2HPO4. 

Nearly  insol.  in  H2O.  (Gmelin.)  Sol.  in 
833  pts."H2O  at  12°.  (Rammelsberg.) 

Li5H(PO4)2+H2O.  Sol.  in  200  pts.  H2O. 
(Rammelsberg.) 

Lithium  dihydrogen  phosphate,  LiH2PO4. 

Deliquescent,  and  very  sol.  in  H2O.  (Ram- 
melsberg.) 

Heptaliihium  cfthydrogen  phosphate, 

Li7H2(P04)3. 
+  1H2O,  or  2H2O.     Sol.  in  H2O.     (Ram- 
melsberg.) 

Lithium  pentahydrogen  phosphate, 

LiH5(PO4)2+H2O. 
Deliquescent,  and  sol.  in  H2O. 


,ithium  p?/rophosphate,  Li4P2O7+2H2O. 
(Rammelsberg,  B.  A.  B.  1883.  21.) 

Lithium     manganous      phosphate,     Li3PO4, 

Mn3(PO4)2. 
Min.  Lithiophilite. 

Lithium    potassium     wetaphosphate,     Li2O, 

2K2O,  3P2O5+4H2O. 

As  NH4  comp.  (Tammann,  J.  pr.  1892, 
(2)  46.  443.) 

Lithium  potassium  pz/rophosphate,  Li3KP2O7. 
(Kraut,  A.  1876,  182.  170.) 

Lithium  sodium  phosphate,  3Li2O,  Na2O, 
P205. 

Insol.  in  H2O.  Sol.  in  dil.  acids.  (Ouvrard, 
C.  R.  110.  1333.) 

2Li2O,  Na2O,  2P2O5.    As  above  (Ouvrard.) 

Lithium  sodium  pyrophosphate,  Li2O,  Na2O, 
P2O£. 

5Li20,  Na2O,  3P2O5. 

4Li2O,  6Na2O,  5P2O5.  (Kraut,  "A.  1876, 
182.  168.) 

Magnesium  metaphosphate,  Mg(PO3)2. 

Insol.  in  H2O  or  dil.  acids,  but  sol.  in  H2SO4 
+Aq.  (Maddrell,  A.  61.  62.) 

Not  decomp.  by  very  long  digestion  with 
alkali  carbonates,  or  orthophosphates  +Aq. 
(Fleitmann.) 

Magnesium   dimetaphosphate,  Mg2(P2Oe)2  + 

9H20. 

Insol.  in  H2O;  decomp.  by  acids.  (Fleit- 
mann, Pogg.  78.  259.) 

Magnesium  trimetaph.ospha.te,  Mg3(P3O9)2. 

SI.  sol.  in  cold  H2O,  more  easily  in  hot  H2O. 
When  ignited,  insol.  in  boiling  HCl+Aq. 
(Lindbom.) 

Cryst.  with  12,  or  15H2O. 

Magnesium  tetrametaphosphate,  Mg2P4Oi2. 

Insol.  in  H2O,  somewhat  sol.  in  HCl+Aq. 
More  easily  sol.  in  HNO3+Aq,  especially 
easily  sol.  in  cone.  H2SO4.  (Glatzel,  Dissert. 
1880.) 

+  10H2O.    Sol.  in  70  pts.  H2O.    (Glatzel.) 

Magnesium  or^ophosphate,  Mga(PO4)2,  and 
+5,  or  7H2O. 

1  litre  H2O  dissolves  0.1  g.  ignited 
Mg3(PO4)2  in  7  days,  but  0.205  g.  if  freshly 
precipitated.  (Volcker,  J.  B.  1862.  131.) 

1  1.  H2O  with  2  g.  NaCl  dissolves  75.8  mg.; 
1  1.  H2O  with  3  g.  NaNO3  dissolves  61.9  mg. 
Mg3(PO4)2.  (Liebig,  A.  106.  185.) 

Easily  sol.  in  acids,  except  in  acetic  acid. 
(Schaffner,  A.  60.  145.) 

Easily  sol.  in  H2O  in  presence  of  alkali  salts. 


PHOSPHATE,  MAGNESIUM,  CHLORIDE 


697 


+6}^H2O.  Sol.  in  30  min.  in  diamrnonium 
citrate+Aq  (sp.  gr.  =  1.09);  triammonium 
citrate+Aq  (sp.  gr.  =  1.09)  dissolves  37.5% 
of  the  P2O5.  (Erlenmeyer,  B.  14.  1253.) 

+20H2O.  Sol.  in  10  min.  in  diammonium 
citrate+Aq  (sp.  gr.  =  1.09);  triammonium 
citrate+Aq  (sp.  gr.  =  1.09)  dissolves  23.2% 
of  the  P2O5;  sol.  in  15  min.  in  Y±%  citric  acid 
+Aq.  (Erlenmeyer,  I.  c.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

Magnesium  hydrogen  phosphate.  MgHPO4+ 

7H20. 

Sol.  in  322  pts.  cold  H2O  in  several  days. 
If  heated  to  40°  becomes  milky,  and  separates 
a  precipitate  out  at  100°  of  same  salt,  so  that 
solution  at  100°  contains  only  1  pt.  salt  in  498 
pts.  H2O.  Much  more  sol.  in  H2O  containing 
traces  of  acids,  even  dil.  oxalic  or  acetic  acids. 
(Graham,  Phil.  Mag.  Ann.  2.  20.)  Easily  sol. 
in  H2SO8+Aq.  (Gerland,  J.  pr.  (2)  4.  127.) 

Sol.  in  aqueous  solution  of  Mg  salts,  but 
insol.  in  Na2HPO4+Aq.  (Rose.)  Sol.  in 
sodium  citrate+Aq.  (Spiller.)  When  freshly 
precipitated  it  is  sol.  in  hot  NH4Cl+Aq,  and 
NH4OH+Aq  does  not  completely  reprecipi- 
tate  it;  less  sol.  in  INH4NO3+Aq.  (Brett, 
Phil.  Mag.  (3)  10.  96.)  Insol.  in  alcohol. 
(Berzelius.) 

For  solubility  in  H3PO4,  see  under  MgO. 

+  3^H2O.    (Debray.) 

+H2O.  Easily  sol.  in  dil.  acids,  (de 
Schulten,  C.  R,  100.  263.) 

+3H2O.  SI.  sol.  in  H2O,  easily  in  acids. 
(Stoklasa,  Z.  anorg.  3.  67.) 

+4^H2O.    (Bergmann.) 

+6H2O.    (Debray.) 

Magnesium  tetrahydrogen  phosphate, 
MgH4(P04)2. 

Not  hygroscopic.  Sol.  in  5  pts.  H2O  with- 
out decomp.  (Stoklasa,  Z.  anorg.  3.  67.) 

+2H2O.  Not  hygroscopic.  Sol.  in  H2O 
without  decomp.  (Stoklasa,  Z.  anorg.  1.  307.) 

Decomp.  by  alcohol  into  MgHPO4+3H2O 

Magnesium  pyrophospnate,  Mg2P2O7. 

Nearly  insol.  in  H2O;  readily  sol.  in  HC] 
or  IINO3+Aq.  (Fresenius.) 

+3H2O.  SI.  sol.  in  H2O,  easily  in  HC1  or 
HNO3+Aq;  sol.  in  H2SO3+Aq,  and  Na4P2O7 
+Aq.  (Schwarzenberg.) 

Sol.  in  MgSO4+Aq,  and  (NH4)2CO3+Aq 

Magnesium  te/raphosphate,  Mg3P4Oi3. 

Insol.  in  H2O.  (Fleitmann  and  Henneberg 
A.  65.  331.) 

Magnesium  potassium  dimefaphosphate, 
K2Mg2(P206)3. 

Very  sol.  in  dil.  acids.  (Ouvrard,  C.  R 
1888,  106.  1729.) 

+4H2O.    Sol.  in  10.2  pts.  H2O.    (Glatzel.; 


Magnesium   potassium  or^ophosphate. 

MgKP04. 

SI.  sol.  in  H2O.    Decomp.  by  H2O.    Easily 
ol.  in  acids. 
+6H2O. 

2MgO,  K2O,  3P2O5.    Insol.  in  H2O;  sol.  in 
dil.  HCl+Aq.     (Ouvrard,  C.  R.  106.  1729.) 
Mg2HK(PO4)2  +  15H20.    (Haushofer.) 

Magnesium  rubidium  or^ophosphate, 
RbMgPO4+6H2O. 

Easily  sol.  in  warm  dil.  HCl+Aq. 

Not  decomp.  by  boiling  H2O.  (Erdmann, 
A.  1897,  294.  73.) 

Magnesium  sodium  ^nphosphate, 

MgNa3P3Oio+13H2O. 
Decomp.  in  the  air.     (Stange,  Z.  anorg. 
1896,  12.  454.) 

Magnesium  sodium    metophosphate,  3MgO, 

Na2O,  4P2O5. 

Insol.  in  H2O  or  H3PO4+Aq.  Scarcely  sol. 
in  HCl+Aq,  or  aqua  regia.  Not  decomp.  by 
(NH4)2CO3+Aq.  Sol.  in  cone.  H2SO4. 
(Maddrell,  A.  61.  53.) 

Magnesium  sodium  dwietaphosphate, 

MgNa2(P2O6)2+4H2O. 
Sol.    in  25  pts.  H2O.     (Glatzel,    Dissert. 
1880.) 

Magnesium  sodium  /n'metophosphate, 

MgNa4(P3O9)2+5H2O. 
SI.  sol.  in  H2O.    After  ignition  is  insol.  in 
H,O.    (Lindbom.) 

Magnesium     sodium     phosphate,     lOMgO, 

8Na2O,  9P2O5. 

Insol.  in  H2O;  easily  sol.  in  dil.  acids. 
(Ouvrard,  C.  R.  106.  1729.) 

Magnesium  sodium  ori/iophosphate, 
MgNaPO4. 

Insol.  in  H2O.    (Rose.) 

+9H2O.  (Schoeoker -and  Violet,  A.  140. 
232.) 

MgO,  2Na2O,  P2O5.  Insol.  in  H2O. 
(Ouvrard.) 

3MgO,  3Na2O,  2P2O5.  Insol.  in  H2O. 
(Ouvrard.) 

Magnesium  sodium  p?/rophosphate,  basic  (?). 

"Precipitate;  si.  sol.  in  H2O.  Easily  in  HC1+ 
Aq,  HNO3+Aq,  and  Na4P2O7+Aq.  (Baer, 
Pogg.  75.  168.) 

Sol.  in  (NH4)2CO3+Aq,  and  in  MgSO4  + 
Aq. 

Insol.  in  alcohol. 

Magnesium  phosphate  chloride,  Mg3(PO4)2, 

MgCl2. 
(Deville  and  Caron,  A.  ch.  (3)  67.  455.) 


698 


PHOSPHATE,  MAGNESIUM,  NITROGEN  OXIDE 


Magnesium  pyrophosph&te  nitrogen  dioxide 

Mg,P,07,  H20,  N02. 
Scarcely  sol.  in  water.    (Luck,  Z.  anal.  13, 
255.) 

Magnesium  phosphate  fluoride,  Mg3(PO4)2) 

MgF2. 

Min.  Wagnerite.  Slowly  sol.  in  hot  HNO3, 
and  H2SO4. 

Magnesium   phosphate    calcium    fluoride, 

2Mg3(P04)2,  CaF2. 
Min.    Kjerulfite. 

Manganous  dimetaphosphate,  Mn2(P2O6)2. 

Anhydrous.  Insol.  in  H2O  and  dil.  acids. 
(Fleitmann.)  Sol.  in  cone.  H2SO4.  (Mad- 
drell.)  Scarcely  attacked  by  warm  Na2S  + 
Aq,  and  not  much  more  by  (NH4)2S+Aq. 
Decomp.  by  Na2CO3+Aq. 

-f-8H2O.  Insol.  in  H2O  and  dil.  acids. 
(Fleitmann,  Pogg.  78.  257.) 

Manganous  trimeiaphosphate,  Mn3(P3O9)2  + 

11H2O. 

Difficultly  sol.  in  cold  or  warm  H2O.  More 
easily  sol.  in  cold,  very  easily  in  warm  HC1  + 
Aq.  When  ignited,  is  insol.  in  acids,  even 
aqua  regia.  (Lindbom.) 

Manganous  hexametaphosphate. 

Sol.  in  sodium  hexametaphosphate +Aq. 
(Rose,  Pogg.  76.  4.) 

Mn3P6Oi8.  Nearly  insol.  in  H2O;  easily 
sol.  in  acids.  (Liidert,  Z.  anorg.  5.  15.) 

Manganic  raetaphosphate,  Mn(PO3)3. 

Insol.  in  H2O  or  acids;  decomp.  by  alkalies. 
(Schjerning,  J.  pr.  (2)  45.  515.) 

Insol.  in  II 2O;  sol.  in  HC1;  decomp.  by 
alkalies +Aq.  (Barbier,  C.  R.  1902,  135. 
1055.) 

+H2O.  Insol.  in  H2O  or  acids,  except 
HCl+Aq.  SI.  decomp.  by  boiling  with 
H2SO4.  (Hermann,  Pogg.  74.  303.) 

Manganous  tetrametaphosphate,  Mn2(PO3)4. 

Not  attacked  by  acids.  (Glatzel,  Dissert. 
1880.) 

+  10H2O.  Sol.  only  in  boiling  cone. 
H2S04.  (Glatzel.) 

Manganous  (Mawetaphosphate, 

5MnO,  5P2O5+12H2O. 
Ppt.      (Tammann,    J.    pr.    1892,    (2)    45. 
450.) 

Manganous  ort/iophosphate,  Mn3(PO4)2. 

+H2O.     (Debray.) 

+3H2O.  Sol.  in  20  min.  in  diamonium 
citrate + Aq  (sp.  gr.  =  1 ,09) ;  triammonium 
citrate+Aq  (sp.  gr.  =  1.09)  dissolves  30.2% 
of  the  P2O5.  (Erlenmeyer,  B.  14.  1253.) 


2O.  Efflorescent.  (Erlen- 
meyer and  Heinrich,  A.  190.  208.) 

+7H2O.  Very  si.  sol.  in  H2O.  (Berzelius.) 
Easily  sol.  in  mineral  acids;  sol.  in  HC2H3O2 
+Aq. 

Easily  sol.  in  SO2+Aq.  (Gerland,  J.  pr. 
(2)  4.  97.) 

Somewhat  sol.  in  boiling  (NH4)2CO3+Aq, 
but  deposited  on  cooling.  (Berzelius.) 

Partly  sol.  in  cold  NH4C1,  or  NH4NO3+Aq. 
(Brett.) 

Sol.  in  cold  or  hot  solutions  of  ammonium 
sulphate  or  succinate.  (Wittstein.) 

SI.  sol.  in  Mn  salts +Aq.  (Rose,  Pogg.  76. 
25.) 

Insol.  in  alcohol. 

Sol.  in  10  min.  in  diarnmonium  citrate+Aq 
(sp.  gr.  =  1.09);  triammonium  citrate+Aq 
(sp.  gr.  =  1.09)  dissolves  53%  of  the  P2O5. 
(Erlenmeyer,  B.  14.  1253.) 

Manganous    c&hydrogen    orthophosphate, 
MnHPO4+3H2O. 

SI.  sol.  in  H2O.  Solution  decomp.  at  100°. 
(Debray.)  Slowly  decomp.  by  cold  H2O  into 
Mn3(PO4)2.  (Erlenmeyer  and  Heinrich,  A. 
190.  203.) 

Easily  sol.  in  H2SO3  +  A.q.    (Gerland.) 

SI.  sol.  in  HC2H3O2,  easily  in  cone,  mineral 
acids.  (Heintz.)  Sol.  in*  (NH4)oCO3+Aq, 
from  which  it  is  repptd.  on  boiling.  Decomp. 
by  boiling  KOH+Aq. 

Insol.  in  alcohol. 

Mn3(PO4)»,  2MnHPO4+4H2O.  (de  Schul- 
ten,  C.  C.  1905, 1.  188.) 

Manganous  te^rahydrogen  phosphate, 
MnH4(PO4)2+2H2O. 

Deliquescent.  Easily  sol.  in  H2O,  with 
decomp.  to  MnHPO4.  (Erlenmeyer  and 
Heinrich,  A.  190.  208.) 

Not  decomp.  by  H2O.  (Otto,  C.  C.  1887. 
1563.) 

H2O  decomp.  it  into  MnHPO4  and  H3PO4 
containing  some  dissolved  salt.  The  less 
H2O  used,  the  more  MnHPO4  separates.  The 
acid  nitrate  separates  MnHPO4  on  boiling. 
A.t  0°  the  decomp.  increases  in  proportion 
to  the  amt.  of  salt,  but  1  g.  of  the  salt  is  un- 
changed in  100  g.  H2O.  With  less  than  20  g. 
of  salt  to  100  g.  H2O  the  decomp.  is  analogous 
to  that  of  CaH4(PO4)2,  but  with  larger  amts. 
of  salt  it  is  the  opposite,  becoming  less  with 
ncreasing  amts.  of  the  salt.  (Viard,  C.  R. 
1899,  129.  412.) 

Alcohol  dissolves  out  H3PO4.     (Heintz.) 

Pentomanganous  c&hydrogen  phosphate, 

Mn6H2(PO4)4+4H2O. 
Not   decomp.    by   boiling   H2O.      (Erlen- 
meyer and  Heinrich,  A.  190.  208.) 

Manganic  or/Aophosphate,  basic,  Mn2P3O8  + 

H2O. 
SI.  sol.  in  H2O. 


PHOSPHATE,  MERCUROUS 


699 


Manganic  orf/iophosphate,  MnPO4+H2O. 

Sol.  in  acids.  (Christensen,  J.  pr.  (2) 
28.  1.) 

Manganous  p?/rophosphate,  Mn2P2O7. 

Anhydrous.  (Lewis,  Sill.  Am.  J.  (3)  14. 
281.) 

+H2O. 

H-3H2O.  Insol.  in  H2O.  Insol.  in  MnSO4  + 
Aq,  but  sol.  in  Na4P2O7+Aq.  (Rose.) 

Difficultly  sol.  in  Na4P2O7+Aq,  but  easily 
sol.  in  K4P2O7+Aq.  (Pahl.)  Decomp.  by 
KOH+Aq.  Sol.  in  H2SO3+Aq.  (Schwar- 
zenberg.) 

Insol.  in  acetone.  (Naumann,  13.  1°-04,  37. 
4329.) 

Manganous  hydrogen  p^ophosphate, 

MnH2P2O7+4H2O. 
Sol.  inII2O.    (Pahl.) 


pyrophosphate, 
;O21  +  14H,O. 


Manganic 
Mn4P 

Sol.  in  H2SO4,  and  H3PO4.  (Auger,  C.  R. 
1901,  133.  95.) 

MnHP2O7.  Insol.  in  H2O;  very  si.  at- 
tacked by  dil.  HCl+Aq,  easily  by  cone.  Sol. 
in  cone.  H2SO4.  (Sehjerning,  J.  pr.  (2)  46. 
515.) 

Manganous  potassium  cfo'metaphosphate. 

K2Mn(PO3)4+6H!JO. 

Sol.  in  95  pts.  H2O.  When  ignited  is  not 
attacked  by  acids.  (Glatzel,  Dissert.  1880.) 

Manganous  potassium  ort/zophosphate, 

Insol.  in  H2O;  easily  sol.  in  dil.  acids. 
(Ouvrard.) 

Manganic    potassium    pyrophosphate, 
MnKP2O7. 

+5H2O.    SI.  sol.  in  cold  H,O. 

+3H2O.  SI.  sol.  in  cold  H2O.  (Rosen- 
heim,  B.  1915,  48.  584.) 

Manganous  potassium  phosphate,  MnK2P2O7 
Insol.  in  H2O;  sol.  in  dil.  acids.     (Ouvrard 

C.  R.  106.  1729.) 

+8H2O.    SI.  sol.  in  H2O.    (Pahl.) 


Mri,P2O7,    2K4P2O7  +  10H2O. 
sol.  in  H2O.    (Pahl.) 


Difficultly 


Manganic    potassium  p?/r0phosph.ate, 

MnKP2O7. 

Insol.   in   H2O.     Decomp.   by   acids   ami 
bases.     (Schjerning.) 

iganic    silver    pyrop 
AgMnP2O7+3H2O. 
Almost   insol.    in   H2O.      (Rosenheim,    B 
1915,  48.  585.) 


Manganous  sodium  ^phosphate, 

MnNa3P3O10+12H2O. 
SI.  sol.  in  H2O;  the  melt  obtained  by  heating 
the  salt  is  readily  sol.  in  H2SO4.     (Stange,  Z. 
anorg.  1896, 12.  455.) 

Manganous  sodium  dimetaphosphate, 

MnNa2(PO3)i+6H2O. 
Easily  sol.  in  boiling  H2SO4,  but  not  at- 
tacked   by    acids    after    boiling.      (Glatzel, 
Dissert.  1880.) 

Manganous  sodium  ^nmetaphosphate, 

Sol.  in  H2O.     (Fleitmann  and  Henneberg.) 
MnNa(PO3)3.    Insol.  in  H2O,  dil.  acids,  or 

alkalies.    (Schjerning,  J.  pr.  (2)  45.  515.) 

Manganous  sodium  ocforaetaphosphate, 
Mn3Na2(PO3)8 

Insol.  in  acids  except  cone.  H2SO4.  (Tam- 
mann,  J.  pr.  1892,  (2)  45.  469.) 

+5H2O.     Almost  insol.  in  cold  H2O. 

Decomp.  by  boiling  H2O  with  separation 
of  Mn2O3.  (Rosenheim,  B.  1915,  48.  584.) 

Manganous    sodium    or^ophosphate. 

MnNaPO4. 

Insol.  in  H2O.    (Ouvrard,  C.  R.  106.  1729.) 
MnO,  2Na2O,  P2O5.    As  above. 

Manganous  sodium  pz/rophosphate, 
MnNa2P2O7. 

Insol.   in   H2O;    easily   sol.   in   dil.   acids. 

(Wallroth.) 

+43^H2O.     Very  si.  sol.  in  H2O.     (Pahl.) 
3Mn2P2O7,    2Na4P2O7+24H2O.      Very   si. 

sol.inH2O.    (Pahl.) 

Manganic  sodium  p?/rophosphate,  MnNaP2O7 

+H2O. 
(Christensen,  J.  pr.  (2)  28.  1.) 

Manganic  dipyrophosphate  ammonia, 
Mn2P4O14,  2NH3. 

Insol.  in  H2O. 

Decomp.  by  HC1  and  by  alkalies.  (Bar- 
bier,  C.  R.  1902,  135.  1109.y 

Manganous  phosphate  chloride,  Mn3(PO4)2, 
MnCl2. 

Insol.  in  H2O.  (Deville  and  Caron,  A.  ch. 
(3)  67.  459. 

3Mn3(PO4)2,  MnCl2.  Insol.  in  H2O.  (De- 
ville and  Caron.) 

Mercurous  /iexawetaphosphate  (?). 

Ppt.  Sol.  in  sodium  hexametaphosphate 
+Aq.  (Rose.) 

Hg6P6O]8.  Insol.  in  H2O;  very  si.  sol.  in 
acids.  (Liidert,  Z.  anorg.  5. 15.) 

Moderately  sol.  in  H2O  when  freshly  pptd. 
More  sol.  in  acids  than  the  mercurous  salt. 
(Liidert.) 


700 


PHOSPHATE,  MERCUROUS 


Mercurous  on'/iophosphate,   (Hc,3)2(PO4)2. 

Ppt.  Decomp.  by  boiling  with  H2O.  (Ger- 
hardt.) 

Sol.  in  HNOs+Aq.  Sol.  in  Hg2(NO3)2  + 
Aq.  Insol.  in  H3PO4+Aq. 

Mercuric  ortfiophosphate,  Hg3(PO4)2. 

Insol.  in  H2O.  SI.  sol.  in  hot  H2O,  crystal- 
lizing out  on  cooling.  (Haack,  A.  262.  185. 
Slowly  sol.  in  cold  dil.,  quickly  in  hot  dil.  or 
cold  cone.  HCl  +  Aq.  Less  easily  sol.  in 
HNO3+Aq.  Sol.  in  H3PO4+Aq.~  (Berze- 
lius.)  InsDl.  in  H3PO4+Aq.  (Haack.)  De- 
comp. by  NaCl+Aq  into  insol.  HgCl2, 
3HgO,  but  sol.  in  NaCl+Aq,  containing 
HNO3.  (Haack.) 

Sol.  in  6  pts.  NH4C1  in  aqueous  solution  by 
heating.  (Tromrnsdorff.) 

Sol.  in  (NH4)2CO3,  (NH4)2SO4,  or  NH4NO3 
+Aq.  (Wittstein.) 

Insol.  in  alcohol. 

Mercuromercuric  ort/iophosphate,  7Hg2O, 

14HgO,  2P2O5+20H2O. 
(Brooks,  Pogg.  66.  63.) 

Mercurous  p?/rophosphate,  Hg4P2O7+H2O. 

Sol.  in  Na4P2O7+Aq,  when  recently  pptd. 
Insol.  in  Na4P2O7+Aq,  when  heated  to  100°. 
Sol.  in  HNO3+Aq.  Decomp.  by  HCl+Aq. 
(Schwarzenberg,  A.  65.  133.) 

Mercuric  ?«/r0phosphate,  Hg2P2O7. 

Sol.  in  acids;  insol.  in  Na4P2O7+Aq,  after 

being  heated  to  100°.      Sol.  in  NaCl+Aq; 

quickly     decomp.     bv     NaOH+Aq,      and 

Na2HPO4+Aq. 

Sol.  in  6  pts.  NH4Cl+Aq.    (Trommsdorff.) 
Sol.  in  NH4NO3,(NH4)SO4,  and  (NH4)2CO3 

+Aq;  also  in  KI+Aq. 

Mercurous  silver  ort/iophosphate,  AgHg2PO4. 
Sol.  in  HNO3.    (Jacobsen,  Bull.  Soc.  1909, 
(4)  6.  949.) 

Molybdenum   phosphate,   Mo2(PO4)2    (?). 
Insol.  in  H2O.    Sol.  in  MoCl2+Aq. 

Molybdenum    sodium   p^/rophosphate, 

Na(MoP2O7)  +  12H20. 
Ppt,     (Rosenheim,  B.  1915,  48.  589.) 

Nickel  dimetaphosphsLte,  NiP2O3. 

Insol  in  H2O  or  dil. acids.  Sol.  in  cone. 
H2SO4.  Not  decomp.  by  boiling  alkali  car- 
bonates or  sulphides  +  Aq.  (Maddrell, 
A.  61.  58. 

+4H2O.  Sol.  in  cold  acids.  (Glatzel, 
Dissert.  1880.) 

Nickel  Zdraraetaphosphate,  Ni2P4O12. 

Insol.  in  HC1.  Sol.  in  cone.  HNO3  and 
especially  sol.  in  H2SO4  on  boiling.  (Glatzel.) 


Nickel  telrametaphosphate,  Ni2P4Oi2  + 

12H2O. 
Easily  sol.   in  acids.      (Glatzel.) 

Nickel  ortfiophosphate,  Ni3(PO4)2+7H2O. 

Insol.  in  H2O.  Sol.  in  acids.  (Rammesl- 
berg,  Pogg.  68.  383.) 

Sol.  in  Ni  salts +Aq.  (Rose,  Pogg.  76. 
25.) 

Insol.  in  NaoHPO4+Aq.    (Tupputi,  1811.) 

Very  si.  sol.  in  hot  (NH4)2HPO4+Aq. 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethylacetate.  (Naumann, 
B.  1910,  43.  314.) 

Nickel  pyrophosphate,  Ni2P2O7+6H2O. 

Insol.  in  H2O;  sol.  in  mineral  acids,  Na4P2O7 
+Aq,  and  NH4OH+Aq.  Not  pptd.  from 
Ni2P2O7  +  Aq  by  alcohol.  (Schwarzenberg, 
A.  65.  158.) 

Nickel  potassium  cfometaphosphate, 

NiK2P4O12+6H2O. 
Sol.  in  130  pts.  H2O.    (Glatzel.) 

Nickel  potassium  or^ophosphate,  NiKPO4. 

Insol.  in  H2O;  sol.  in  dil.  acids.  (Ouvrard, 
R.  106.  1729.) 

3NiO,  3K2O,  2P2O6.    As  above. 

Nickel  sodium  ^nphosphate,   Na3NiP3O19  + 

12H2O. 

Very  sol.  in  H2O;  decomp.  in  Aq  solution. 
(Schwarz,  Z.  anorg.  1895,  9.  261.) 

Nickel  sodium  meta phosphate,  3Ni(PO3)2, 
NaPO3. 

Insol.  in  H2O  and  dil.  acids.  Sol.  in  cone. 
H2SO4.  (Maddrell,  A.  61.  56.) 

NiNa4(PO3)3+8H2O.  Easily  sol.  in  H2O. 
(Lindbom.) 

Nickel  sodium  cfe'raetaphosphate,  NiNa2P4Oi2 

+6H2O. 

SI.  sol.  in  H2O.  Moderately  sol.  in  acids. 
(Glatzel,  Dissert.  1880.) 

Nickel  sodium  ^nmetaphosphate. 
Ni2Na2(P309)2+9H20. 

1  1.  H2O  dissolves  60.6  g.  at  20°.  (Tam- 
mann,  J.  pr.  1892,  (2)  45.  426.) 

Na3NiP3Oio4-12H2p.  Insol.  and  not  de- 
comp. by  H2O.  Sol.  in  acids.  (Schwarz,  Z. 
anorg.  1895,  9.  261.) 

Nickel  sodium  octoraetaphosphate, 

Na2Ni3(PO3)8. 
(Tammann,  J.  pr.  1892,  (2)  45.  469.) 

Nickel  sodium  or^ophosphate,  NiNaPO4+ 
7H20. 

Ppt.    (Debray,  C.  R.  59.  40.) 

NiO,  2Na2O,  P2O5.  Insol.  in  H2O.  Easily 
sol.  in  dil.  acids.  (Ouvrard.) 


PHOSPHATE,  POTASSIUM  HYDROGEN 


701 


Nickel  sodium  pi/rophosphate, 

Ni10Na]fi(P2O7)9. 

Insol.  in  H2O.  Moderately  sol.  in  acids. 
(Wallroth.) 

Osmium  phosphate  (?). 

SI.  sol.  in  H2O;  sol.  in  HNO8+Aq.  (Ber- 
zelius.) 

Palladium  or^Aophosphate  (?). 
Ppt, 

Phosphorus  phosphate,  4P4O,  3P2O5  (?). 

Decomp.  spontaneously.  Sol.  in  H2O  and 
alcohol  when  fresh;  insol.  in  ether,  (le  Verrier, 
A.  27.  167;  Reinitzer,  B.  14.  1884.) 

Platinum  phosphate,  PtP2O7. 

Insol.  in  H2O,  acids  and  alkalies.  Decomp. 
by  fusing  with  potassium  carbonate.  (Bar- 
nett,  C.  N.  1895,  71.  256.) 

Potassium  raoraowetaphosphate,  KPO3. 

Nearly  insol.  in  H2O;*s3l.  in  weak  acids, 
even  in  acetic  acid.  (Maddrell,  A.  61.  62.) 

Insol.  in  H2O  and  weak  acids.  (Fleitmann, 
Pogg.  78.  250.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Potassium  eftmetaphosphate,  K2P2Oe+H2O. 

Sol.  in  1.2  pts.  cold  H2O,  but  not  more  in 
hot  H2O.  (Fleitmann,  Pogg.  78.  250.) 

Potassium  trimetaphospha.te,  K3P3O9. 

Very  sol.  in  cold  H2O  before  it  is  fused. 
(Lindbom,  Acta  Lund.  1873.  14.) 

Potassium  or^ophosphate,  K3PO4. 

Not  deliquescent.  Very  sol.  in  H2O. 
(Graham,  Pogg.  32.  47.) 

Very  si.  sol.  in  cold,  easily  in  hot  H2O. 
(Darracq.) 

Solubility  in  H3PO4+Aq  at  25°. 


In  1000  g.  of  the  solution,  me 


K 

P04 

9.14 

8.84 
8.42 
7.52 
6.90 
6.88 

3.13 
3.22 
3.44 
3.78 
4.15 
4.12 

(D'Ans  and  Schreiner,  Z.  phys.  Ch.  1910,  76. 
103.) 

Insol.  in  alcohol. 

Potassium  hydrogen  or^ophosphate, 

2K2HP04,  KH2PO4+H2O. 
Very  unstable;  very  sol.  in  H2O  with  de- 
comp.     Identical    with    the    substance    de- 


In  1000  g.  of  the  solution,  mols. 

K 

P04 

6.80 

4.08 

6.80 

4.05 

6.76 

3.96 

6.50 

3.81 

6.16 

3.61 

5.24 

3.25 

4.42 

2.94 

scribed  as  dipotassium  phosphate  by  Ber- 
zelius.  (Staudenmaier,  Z.  anorg.  1894,  6. 
389.) 

3K2HPO4,  KH,PO4+2H2O.  Very  unstable; 
very  sol.  in  H2O  with  decomp.  (Stauden- 
maier.) 

Potassium  hydrogen  or^ophosphate, 

K2HPO4. 
Deliquescent.    Very  sol.  in  H2O  and  alcohol. 

Solubility  in  H3PO4+Aq  at  25°. 


(D'Ans  and  Schreiner,  Z.  phys.  Ch.  1910,  76. 
103.) 

Potassium  cfahydrogen  phosphate,  KH2PO4. 

Deliquescent.  Easily  sol.  in  H2O.  (Vau- 
quelin,  A.  ch.  74.  96.) 

1  1.  sat.  aq.  solution  at  7°  contains  249.9  g. 
KH2PO4.  (Muthmann  and  Kuntze,  Z.  Kryst. 
Min.  1894,  23.  308.) 

Solubility  in  H3PO4+Aq  at  25°. 


In  1000  g.  of  the  solution,  mols. 


K 

P04 

2.90 

2.36 

1.70 

1.71 

1.60 

1.67 

1.48 

1.46 

1.78 

3.15 

2.18 

4.65 

2.54 

6.32 

2.66 

6.76 

2.98 

8.03 

3.32 

8.80 

(D'Ans  and  Schreiner,  Z.  phys.  Ch.  1910,  75. 
103.) 

Sp.  gr.  of  KH2PO4+Aq  at  18°  containing: 

5  10  15%KH,PO4. 

1.0341         1.0691         1.1092 

(Kohlrausch,  W.  Ann.  1879.  1.) 

Sol.  in  20%  KC2H3O2+Aq.  (Strom ever.) 
For  solubility  in  H2O,  see  K2HPO4,  H8PO4. 
Insol.  in  alcohol.* 


702 


PHOSPHATE,  POTASSIUM,  ACID 


Potassium    orthophosphate.    acid.    KH2PO4, 
H3P04. 

Solubility  in  H2O  at  t°. 


t° 

% 

KH2P04,H3P04 

Solid  phase 

—  0.6 

3.337 

Ice 

-  2.5 

12.13 

a 

-  6.7 

29.43 

K 

-  9.2 

36.98 

a 

-13 

44 

Ice+KH2PO4 

0(?) 

45.8 

KH2P04 

+10.9 

50.3 

t( 

65.2 

68.44 

(i 

78 

72.43 

n 

87.5 

77.6 

(i 

105.5 

85.9 

K 

120 

92.1 

"+KH2P04,  H3P04 

135 

96.1 

KH2PO4,  H3PO4 

139 

100 

(i 

(Parravano  and  Mieli,  Gazz.  ch.  it.  38.  II, 
536.) 

Solubility  in  anhydrous  H3PO4  at  t°. 


t° 

%  KH2P04,  H3PO4 

38.5 
84 
110 
126.5 

18.17 
58.42 
77.53 
92.26 

(Parravano  and  Mieli.) 

Potassium  pyrophosphate,  K4P2O7+3H2O. 

Very  deliquescent,  and  sol.  in  H2O. 

Precipitated  from  aqueous  solution  by  al- 
cohol. (Schwarzenberg,  A.  65.  136.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Potassium  hydrogen  pyrophosphate, 

K2H2P2O7. 

Very  deliquescent,  and  sol.  in  H2O.  Insol. 
in  alcohol.  (Schwarzenberg.) 

Potassium  silver  raetaphosphate, 

K2As;4(P03)6+H20. 
(Tamrnann,  J.  pr.  1892,  (2)  45.  417.) 

Potassium  sodium  cfawetophosphate, 

KNaP2O6+H2O. 

Sol.  in  24  pts.  H2O.  (Fleitmann,  Pogg.  78. 
339.) 

Potassium  sodium  phosphate.  KNaHPO4  + 

7H20. 
Not  efflorescent.    Sol.  in  H2O. 

Tnpotassium  ^nsodium  hexahydrogen  phos- 
phate, H6Na3K3(PO4)4-f  22H2O. 
Sol.  in  H2O.    (Filhol  and  Senderens,  O.  R 
93.  388.) 


Potassium  sodium  pyrophosphate, 

K2Na2P2O7  +  12H2O. 
Sol.  in  H2O.    (Schwarzenberg,  A.  65.  140.) 

Potassium  strontium  cftraetaphosphate, 

K2Sr(P2O6)2+4H2O. 
As  the  KBa  comp.    (Glatzel,  Dissert.  1880.) 

Potassium      strontium     hexametaphosphate, 

K2Sr2P6O18. 
(Tammanri,  J.  pr.  1892,  (2)  45.  435.) 

Potassium  strontium  or^ophosphate, 

KSrPO4. 

Insol.  in  H2O;  sol.  in  dil.  acids.  (Grandeau, 
A.  ch.  (6)  8.  193.) 

Potassium  strontium  pyrophosphate, 

K2SrP2O7. 

Insol.  in  H2O;  sol.  in  dil.  acids.  (Ouvrard, 
C.  R.  106.  1599.) 

Potassium  thorium  phosphate,  K2O,  4ThO2, 
3P205. 

Insol.  in  HC1,  HNO3,  or  aqua  regia. 
(Troost  and  Ouvrard,  C,  R.  102.  1422.) 

K2O,  ThO2,  P2O5.  Insol.  in  H2O;  sol.  in 
HNOs+Aq.  (Troost  and  Ouvrard.) 

6K2O,  3ThO2,  4P2O5.  Sol.  in  acids. 
(Troost  and  Ouvrard.) 

Potassium    tin    (stannic)    phosphate,    K20, 

4SnO2,  3P2O6. 
(Ouvrard,  C.  R.  111.  177.) 
K2O,  2SnO2,  P2O5.    (Ouvrard.) 

Potassium  titanium  phosphate,  K2O,  4TiO2, 

3P206. 

(Ouvrard.  C.  R.  111.  177.) 
K2O,  2TiO,>,  P2O5.    (Ouvrard.) 

Potassium  uranous  phosphate,  4UO2,  K2O, 

3P205. 

Practically  insol.  in  cone.  HNO3  and  HC1, 
even  when  the  acids  are  boiling.     Attacked- 
by  HF-f  HNO3.    (Colani,  A.  ch.  1907,  (8)  12. 
133.) 

Potassium     uranous    wetaphosphate,    U02, 

K2O,  P2O5. 

Easily  sol.  in  HNO3.  Sol.  in  cone.  HC1. 
(Colani.) 

Potassium    uranous     pyrophosphate,    SUOz, 

6K2O,  4P2O5. 
Sol.  in  acids.    (Colani.) 

Potassium    uranyl    phosphate,    K2O,    UO3, 

P2O5. 

(Ouvrard,  C.  R.  110.  1333.) 
2K2O,  UO8,  P2O5.    (Ouvrard.) 
K2O,  2UO3,  P2O5.    (Ouvrard.) 


PHOSPHATE,  SILVER 


703 


Potassium   uranyl  or^ophosphate. 

K(UO2)PO4-f3H2O. 
As  NH4  comp.    (Lienau,  Dissert.  1898.) 

Potassium  vanadium  phosphate. 
See  Phosphovanadate,  potassium. 

Potassium  yttrium  phosphate,  3K2O,  Y2O3 

2P2O5. 

K2O,  Y2O3,  2P2O5. 
3K2O,  5Y2O3,  6P2O5.    (Duboin,  C.  R.  107 

622.) 

Potassium  zinc  te/rawetaphosphate, 
K,Zn(PO3)4+6H2O. 

Sol.  in  70  pts.  H2O.  (Glatzel,  Dissert 
1880.) 

Potassium  zinc  phosphate,  KZnPO4. 

Insol.  in  H2O.  Sol.  in  dil.  acids.  (Ouvrard 
C.  R.  106.  1729.) 

K2ZnP2O7.    As  above. 

Potassium  zirconium  phosphate,  K2O,  4ZrO2 
3P2O5. 

Insol.  in  acids  or  aqua  regia.  (Troost  anc 
Ouvrard,  C.  R.  102.  1422.) 

K2O,  ZrO,,  P2O5.  Insol.  in  H2O,  HNO3 
HC1,  or  aqua  regia.  Sol.  in  hot  cone.  H2SO4 
(Troost  and  Ouvrard.) 

Potassium  phosphate  selenate. 
See  Selenophosphate,  potassium. 

Potassium    hydrogen    phosphate    sulphate, 

Decomp.  by  H2O  and  alcohol.  (Jacque- 
lain.) 

Rhodium  phosphate,  basic,  4Rh2O3,  3P2O5-f 
32H2O. 

Insol.  in  H2O  or  acids.    (Glaus.) 
Rh2O3,  P205+6H2O  =  RhPO4+3H2O     Sol 
in  H2O.    (Glaus.) 

Rubidium  metophosphate,  RbPO3. 

Sol.  in  H2O.    (von  Berg,  B.  1901,  34.  4183.) 

Rubidium  or^ophosphate,  Rb3PO4-j-4H2O. 

Hydroscopic;  sol.  in  H2O;  pptd.  by  alcohol, 
(von  Berg,  B.  1901,  34.  4183.) 

Rubidium  hydrogen  or^ophosphate, 

Rb2HP04+H20. 

Sol.  in  H2O;  insol.  in  cone.  NH4OH+Aq- 
insol.  in  alcohol,  (von  Berg.) 

Rubidium    dihydrogen    or/Aophosphate, 
RbHvPO4. 

Very  sol.  in  H2O;  pptd.  by  alcohol,  (von 
Berg.) 


Rubidium  pyrophosphate,  Rb4P2O7. 
Hydroscopic;  sol.  in  H2O.     (von  Berg.) 

Samarium     anhydrometaphosphate,     Sm2O8, 

5P2O6. 
Insol.  in  H2O  or  HNO3+Aq.    (Cleve.) 

Samarium  or^ophosphate,  SmPO4. 

Scarcely  attacked  by  boiling  HNO3+Aq. 
(Cleve.) 

+2H20. 

Samarium  pz/rophosphate,  SmHP2O7+ 
13^H2O. 

(Cleve.) 
Silicon  phosphate. 

See  Silicophosphoric  acid. 
Silver  metophosphate,  Ag2O,  2P2O5+H2O. 

(Kroll,  Z.  anorg.  1912,  76.  408.) 
Silver  cftmetaphosphate,  Ag2P2Oc. 

Very  si.  sol.  in  H2O.  (Fleitmann,  Pogg. 
78.  253.) 

Sol.  in  cold  aniline  metaphosphate-f-Aq. 
(Nicholson.) 

Very  si.  sol.  in  H2O.  (Warschauer,  Dis- 
sert. 1903.) 

+H2O.  Very  sol.  in  H2O.  (Langheld,  B. 
1912,  45.  3760.) 

Silver  Znraetaphosphate,  Ag3P3O9. 

Sol.  in  60  pts.  cold  H2O.  Can  be  crystal- 
lized from  cone.  HNO3+Aq.  (Fleitmann  and 
Henneberg.) 

+H2O.    (Lindbom.) 

Silver  hexametaphosphate,  AgePeOis. 

Insol.  in  H2O.  Sol.  in  HNO3  or  NH4OH  + 
Aq,  and  in  a  large  excess  of  sodium  hexa- 
metaphosphate+Aq.  (Rose.) 

Easily  decomp.  by  Na2S+Aq. 

Decomp.     gradually    by    hot    H?O    into 

When   freshly  pptd.,  easily   sol.  in   H2O. 
Casily  sol.  in  dil.  acids.     (Liidert,  Z.  anorg. 
5.  15.) 

Silver  ort/iophosphate,  Ag3PO4. 

Very  si.  sol,  in  H2O.  1  1.  H2O  dissolves 
6.5  X10-3  g.  Ag3PO4  at  19.46°.  (Bottger,  Z. 
phys.  Gh.  1903,  46.  603.) 

Sol.  in  H3PO4,  HNO3,  or  HC2H3O2+Aq,  in 

\H4OH  or  (NH4)2CO3+Aq.     Less  easily  in 

ammonium  nitrate  or  succinate,  and  incom- 

letely  in   (NH4)2SO4+Aq.      (Lassaigne,   J. 

Pharm.  (3)  16.  289.) 

Insol.  in  Na2HPO4+Aq.     (Stromeyer.) 

Not  pptd.  in  presence  of  Na  citrate. 
Spiller.) 

If  1  mol.  Ag3PO4  is  boiled  with  1  mol. 
\Ta2CO3,  44%  of  it  is  decomp.  (Malaguti.) 

Readily  sol.  in  soluble  hyposulphites +Aq 
ith  decomp.  (Herschel.) 

Insol.  in  Ag  salts  -j-Aq.    (Rose.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
898,  20.  829.) 


704 


PHOSPHATE,  SILVER  HYDROGEN 


Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  "ethyl  acetate.  (Naumann, 
B.  1910,  43.  314.) 

Silver  hydrogen  or^ophosphate,  Ag2HPO4. 

Decomp.  by  H2O  or  alcohol  into  H3PO4  and 
AgaPO4.  (Joly,  C.  R.  103.  1071.) 

Sol.  in  H3PO4+Aq;  insol.  in  ether. 
(Schwarzenberg,  A.  65.  162.) 

Silver  pi/rophosphate,  Ag4P2O7. 

Insol.  in  hot  or  cold  H2O.  Sol.  in  cold 
HNO3+Aq  without  decomp.  Decomp.  by 
hot  HNO3  or  H2SO4  into  orthophosphate. 
Decomp.  by  HCl+Aq  into  AgCl  and  H3PO4. 
Insol.  in  HC2H3O2+Aq.  Sol.  in  NH4OH  + 
Aq  without  decomp.  (Stromeyer,  Schw.  J. 
58.  126.) 

Insol.  in  Na4P2O7+Aq.  Very  si.  sol.  in 
AgNO3+Aq.  (Schwarzenberg,  A.  65.  161.) 

Not  completely  insol.  in  Na4P2O7+Aq. 
(Rose.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 

Silver  hydrogen  pt/rophosphate,  Ag2H2P2O7. 

Decomp.  by  H2O  into  Ag4P2O7.  (Hurtzig 
and  Geuther,  A.  111.  160.) 

Decomp.  by  cold  H2O.  (Cavalier,  C.  R. 
1904,  139.  285.) 

Silver    hydrogen    pT/rophosphate    metaphos- 

phate,  2Ag2HP2O7,  HPO3. 
Decomp.  by  H2O.    Easily  sol.  in  HNO3+ 
Aq.    (BLandG.) 

Silver  ZeJraphosphate,  6Ag2O,  4P2O5  = 
Ag6P4O13. 

Insol.  in,  but  gradually  decomp.  by  boiling 
H2O.  (Berzelius.) 

Sol.  in  large  excess  of  the  corresponding 
Na  salt+Aq. 

Silver  de/caphosphate,  Agi2Pi0O3i. 

Easily  sol.  in  sodium  dekaphosphate+Aq. 
(Fleitmann  and  Henneberg,  A.  65.  330.) 

Silver  ^raphosphate,  Ag2O,  3P2O5. 

(Kroll,  Z.  anorg.  1912,  76.  407.) 
Silver  sodium  dwetaphosphate,  AgNaP2O6. 

Sol.  in  H2O.  (Fleitmann  and  Henneberg, 
Pogg.  65.  310.) 

Silver     sodium    pyrophosph&te,     6Ag4P2O7, 

Na4P2O7+4H2O. 

Not  completely  sol.  in  Na4P2O7+Aq. 
Easily  sol.  in  HNO3+Aq.  (Baer,  Pogg.  75. 
152.) 

Easily  sol.  in  H2O.    (Stromeyer.) 
Ag3NaP2O7  +  KH2O.      ppt.      (Stange,    Z 
anorg.  1896,  12.  460.) 

Silver  uranyl  phosphate,  2Ag2O,  6UO3,  3P2O 

+30H2O. 
(Blinkoff,  Dissert.  1900.) 


Silver  phosphate  ammonia,  Ag3PO4,  4NH3. 

(Widmann,  B.  17.  2284.) 
Sodium  /n'phosphate,  Na5P3Oi0. 

Very  sol.  in  H2O;  decomp.  easily  in  aa. 
solution  at  100°.  (Schwarz,  Z.  anorg.  1895, 
9.  253.) 

Sodium  monoraetaphosphate,  NaPO3. 

Insol.  in  H2O.  Sol.  in  dil.  and  cone,  acids. 
(Maddrell,  A.  61.  63.) 

Insol.  in  acids.    (Graham.) 

Gradually  deoomp.  by  alkalies. 

Sodium  diwetophosphate,  Na2P2O6+2H2O. 

Deliquescent.  Sol.  in  7.2  pts.  of  cold  or  hot 
H2O.  Very  sol.  in  cone.  HCl+Aq.  Sol.  in 
NaOH+Aq.  Insol.  in  strong,  verv  si.  sol.  in 
dilute  alcohol.  (Fleitmann,  Pogg.  78.  246.) 

Sodium  inwetaphosphate,  Na3P3O9+6H2O. 

Sol.  in  4.5  pts.  cold  H2O.  Insol.  in  strong, 
very  si.  sol.  in  dil.  alcohol.  (Fleitmann  and 
Henneberg,  A.  65.  307.) 

Decomp.  by  boiling  H2O.     (Lindbom.) 

Sodium  te/rawetophosphate,  Na4P4OJ2. 

Sol.  in  H2O;  cryst.  with  about  4H2O.  Less 
sol.  in  alcohol  than  in  H2O.  (Fleitmann, 
Pogg.  78.  854.) 

Sodium  heximetaphosphate,  Na6P6Ois. 

Deliquescent.  Very  sol.  in  H2O.  Insol.  in 
alcohol.  (Graham,  Pogg.  32.  56.) 

Sodium  or//iophosphate,  Na3PO4  +  12H2O. 

Not  deliquescent  in  dry  air. 

100  pts.  H2O  dissolve  19.6  pts.  crystals  at  15.5°. 
(Graham.) 

100  pts.  H2O  dissolve  28.3  pts.  Na3PO4+ 
12H2O  at  15°.  (Schiff.) 

Solubility  in  H3PO4+Aq  at  25°. 


In  1000  g.  of  the  solution,  mols. 

Na 

PO4 

4.28 
3.24 
2.24 
2.73 

0.040 
0.183 
0.752 
1.08 

(D'Ans  and  Schreiner,  Z.  phys.  Ch.  1910,  75. 
101.) 

Sp.  gr.  of  Na3PO4+Aq  at  15°. 
=  %Na3P04+12H20. 


% 

Sp.  gr. 

% 

Sp.  gr. 

% 

Sp.  gr. 

1 

2 
3 

4 
5 
6 

7 
8 

.0043 
.0086 
.0130 
.0174 
.0218 
.0263 
.0308 
.0353 

9 
10 
11 
12 
13 
14 
15 
16 

1.0399 
1.0455 
1.0492 
1.0539 
1.0586 
1.0633 
1.0681 
1  .  0729 

17 
18 
19 
20 
21 
22 
23 
24 

1.0778 
1.0827 
1.0876 
1.0925 
1.0975 
1.1025 
1.1076 
1.1127 

(Schiff,  calculated  by  Gerlach,  Z.  anal.  8.  280.) 

PHOSPHATE,  SODIUM 


705 


InsoL  in  CS2.     (Arctowski,  Z.  anorg.  1894 

6O£\7    \ 

Solubility  in  H20  at  t°. 

•  AOl  .) 

Insol.  in  methyl 

acetate.     (Naumann,  B 

t° 

G.  Na2HPO4  in  100  g.  H2O 

1909.  42.  3790.) 

+10H2O.    (Rammelsberg.) 

10.26 

3.55 

Could  not  be  obtained.     (Hall,  J.  pr.  94 

237) 

25.15 
40.29 

12.02 

54.88 

+7H2O.    (Hall.) 
Melts  in  crystal  water  at  76.6°.    (Graham. 

60.23 
99.77 

83.00 
102.15 

Sodium  hydrogen  phosphate,  Na2HPO4. 

Three  breaks  in  the  curve:  at  36.45°,  transi- 

Sol. in  H2O  with  evolution  of  heat. 
100  pts.  H2O  dissolve  at  t°. 

tion    from  dodecahydrate  to   heptahydrate; 
.at  48°,  transition  from  heptahydrate  to  the 
dihydrate;  at  95.2°,  transition  from  dihydrate 
to  the  monohvdrate.     (Shiomi,  C.  C.  1909, 

to 

Pts. 

4.0 

PtS.                    ,o 

Pts. 

Na2HP.O4 

.  

t 

Na2HPO4 

NazHPO 

II.  106.) 

0 
10 
on 

1.55 
4.10 
1  1  no 

40 
50 

ftfl 

30.88           80 
43.31            90 

K  pr   OO                 1  nn 

81.29 
95.02 
i  no  on 

Solubility  of  Na2HPO4  in  H2O  at  t°. 

4U 

30 

1  .l.Uo 
19.95 

ou 
70 

oo.^y         iuu 
68.72          106.2 

lUo.^U 

114.43 

t° 

G.  Na2HP04 
in  100  g.  H2O 

Solid  phase 

(Poggiale,  J.  Pharm.  (3)  44.  273.) 

100  pts.    H2O   at    13°   dissolve   3.4   pts.    NaaHPO 

—0.43 

1.42 

Ice 

(Ferein,  Ph.  Viertelj.  7.  244);  at  15°,  5.9  pts.  (Neese) 
at  16°,  6.3  pts.  (Mulder);  at  16°,  8.4  pts.  (Miiller,  J 

-0.24 

OPak 

0.70 

M 

pr.  95.  52)  ;  at  20°,  6.8  p 

ts.  (Neese,  Russ.  Z.  Pharm.  1 

.5* 

101);  at  25°,  12.5  pts.  (ibid.). 

+0.05 

1.67 

Na2HPO4+12H2O 

Solubility  in  100  pts.  H2O  at  t°. 

20.0 
25  0 

7.66 
12  0 

« 
u 

Pts. 

,o 

Pts. 

Pts. 

32!  o 

J-^f  .  \J 

25.7 

(i 

t 

Na2HPO 

t 

Na2HPO 

t 

Na2HPO4 

34.0 

33.8 

ii 

0 
1 

2.5 
2.6 

35 

36 

39.3 
43.6 

69 
70 

94.8 

95.0 

35.2* 
39.2 

AK.    0 

51.8 
fi7  ^ 

Na2HPO4+7H2O 

t( 

2 

2.6 

37 

49.5 

71 

95.1 

T:O  .  \J 
4.C    Q* 

U  i  .  O 

3 

4 

2.7 
•  2.7 

38 
39 

55.5 
60.6 

72 
73 

95.2 
95.4 

rrO  .  O 

50.0 
fiO  0 

80.2 

Na2HPO4+2H2O 

5 

2.8 

40 

63.9 

74 

95.6 

v/v/  •  U 

80  0 

Q9   Q 

tt 

6 

3.0 

41 

66.2 

75 

95.8 

Oly  .  \J 

on  0 

O--I  .   t/ 

oo  4 

(i 

7 

3.2 

42 

68.6 

76 

96.0 

t/U  •  \J 

of;* 

*->&  .  Tt 

10T  0 

te 

8 
9 
10 

3.4 
3.6 
3.9 

43 
44 
45 

70.8 
72.9 

74.8 

77 
78 
79 

96.1 
96.3 
96.5 

J7t_| 

96.2 

105.0 
ion 

J.U.1  •  \J 

104.6 
102.3 

QQ  9 

Na2HP04 
11 

n 

11 

4.2 

46 

76.5 

80 

96.6 

\.£i\j 

yif  .  £i 

12 
13 
14 
15 

4.5 
4.9 
5.3 

5.8 

47 

48 
49 
50 

78.2 
79.7 
81.2 

82.5 

81 
82 
83 
84 

96.8 
96.9 
97.0 
97.1 

(Menzies  and  Humphery,  Int.  Cong.  App. 
Chem.  1912,  2.  177.) 
*  Transition  points. 

16 
17 

6.3 
6.9 

51 
52 

83.7 
84.8 

85 
86 

97.2 
97.4 

Solubility  in  H2O  at  t°. 

18 

7.6 

53 

85.8 

87 

97.5 

100  g.  H2O 

19 

8.4 

54 

86.7 

88 

97.6 

t° 

dissolve  g. 

Solid  phase 

20 

9.3 

55 

87.7 

89 

97.7 

Na-sHPO 

21 

22 

10.3 
1.1.4 

56 
57 

88.6 
89.4 

90 
91 

97.8 
97.9 

0° 
25 

2.51 
10  47 

Na2HP04,  12H20 

(t 

23 
24 

12.6 
14.0 

58 
59 

90.2 
90.9 

92 
93 

98.0 
98.1 

35.4* 
40  3 

±£l  •  TC  / 

46.11 

K.A     QfJ 

Na2HP04,  7H20 
n 

25 
26 

15.4 
16.9 

60 
61 

91.6 
92.2 

94 
95 

98.2 
98.4 

^t\J  •  O 

48.35* 

KQ    7 

UTC  .  <j\J 

79.00 

Of    q 

Na2HPO4,  2H20 

27 

18.5 

62 

92.7 

96 

98.5 

Ot7  .    1 

71 

yi  .  o 

QK     1 

28 

20.2 

63 

93.1 

97 

98.6 

*  L 

Q1 

c/0  .  1 
OQ     1  K 

29 

22.0 

64 

93.5 

98 

98.7 

*7  A                                            C7CJ  .  JUJ 

30 
31 

24.1 
26.4 

65 
66 

93.8 
94.1 

99 
105 

98.8 
82.5 

D'Ans  and  Schreiner.   Z.  phys.  Ch.  1911. 
75.  99.) 

32 
33 

29.1 
32.1 

67 

68 

94.4 
94.6 

105.57 
106.4 

80.7 
79.2 

*Transition  points. 

34 

35.5 

... 

The  composition  of  the  hydrates  formed  by 
;his  salt  at  different  dilutions  is  calculated 

(Mulder,  Scheik.  Verhandel.  1864.  103.) 

706 


PHOSPHATE,  SODIUM  HYDROGEN 


from  determinations  of  the  lowering  of  the  fr.- 
pt.  produced  by  the  salt  and  of  the  conductiv- 
ity and  sp.  gr.  of  its  aqueous  solutions.  (Jones, 
Am.  Ch.  ,1/1905,  34.  318.) 
Na2HPO4+Aq  saturated  at  15°  has  1.0469 
sp.  gr.    (Michel  and  Krafft)  ;  saturated  at  16°, 
1.0511  (Stolba). 

Sp.  gr.  of  Na2HPO4+Aq  at  19°. 

Solubility  in  H3PO4+Aq  at  25°. 

In  1000  g.  of  the  solution,  mols. 

Na 

P04 

6.31 
6.76 
7.31 

4.63 
4.88 
5.55 

(D'Ans  and  Schreiner,  Z.  phys.  Ch.  1910,  76. 
101.) 
See  also  above. 

4-12H2O.    Efflorescent.    Sol.  in  H2O  with 
absorption  of  heat. 
14  pts.  Na2HPO4+12H2O  mixed  with  100 
pts.  II2O  at  10.8°  lower  the  temperature  3.7°. 
(Riidorff,  B.  2.  68.) 

Sol.  in  8.48  pts.  H2O  at  17°,  or  100  pts.  H2O  dissolve 
11.8  pts.  at  17°,  and  solution  has  sp.  gr.  =  1.0422.  (Schiff  .) 
Sol.  in  4  pts.  cold,  and  2  pts.  boiling  H2O.     (Pagens.) 
Sol.  in  4  pts.  H2O  at  18.75°.     (Abl.) 
100  pts.  H20  dissolve  12.735  pts.  Na2HPO4  +  12H2O. 
(Michel  and  Krafft.) 

%  NaaHPO* 
+12H20 

Sp.  gr. 

%  Na2HP04 
+12H2O 

Sp.  gr. 

fa 

II 

&s 

Sp.  gr. 

1 

2 
3 

4 

1.0041 
1.0083 
1.0125 
1.0166 

5 
6 

7 
8 

1.0208 
1.0250 
1.0292 
1.0332 

9 
10 
11 
12 

1.0376 
1.0418 
1.0460 
1.0503 

(Kf^hiff    A    110   70  ^ 

Saturated  solution  freezes  at  — 0.45°  (Rii- 
dorff,  Pogg.  122.  337),  and  boils  at  105° 
(Griffiths),  105-106.4°  (Mulder),  108.5°  (Le- 
grand). 

Sat.  Na2HPO4+Aq  boils  at  105.5°  (Grif- 
fiths); at  106.5°,  and  contains  113.2  pts. 
Na2HPO4  to  100  pts.  H2O  (Legrand);  forms  a 
crust  at  106.4°,  and  contains  108.8  pts. 
Na2HPO4  to  100  pts.  H2O;  highest  temp,  ob- 
served, 106.8°.  (Gerlach,  Z.  anal.  26.  427.) 


B.-pt.  of  Na2HPO4-f-Aq  containing  pts. 
Na2HPO4  to  100  pts.  H2O.  G  =  accord- 
ing to  Gerlach  (Z.  anal.  26.  450);  L  = 
according  to  Legrand  (A.  ch.  (2)  59.  426.) 


B.-pt. 

G 

L 

B.-pt. 

G 

L 

100.5° 

8.6 

11.0 

104° 

68.4 

76.4 

101 

17.2 

21.0 

104.5 

76.9 

84.2 

101.5 

25.8 

31.0 

105 

85.3 

91.5 

102 

34.4 

40.8 

105.5 

93.7 

98.4 

102.5 

42.9 

50.3 

106 

102.1 

105.0 

103 

51.4 

59.4 

106.5 

110.5 

111.4 

103.5 

59.9 

68.1 

106.6 

112.6 

-fH2O.    Transition  point,  95.2°.    (Shiomi.) 

-r-2H2O.  Transition  point,  48.35°.  (D'Ans 
and  Schreiner);  48°  (Shiomi);  48.3°  (Menzies 
and  Humphery). 

+7H2O.  Not  efflorescent.  Sol.  in  H2O 
with  absorption  of  heat. 

Sol.  in  8  pts.  H2O  at  23°.  (Neese,  J.  B. 
1863.  181.) 

Transition  point,  35.4°  (D'Ans  and 
Schreiner);  36.45°  (Shiomi);  35.2°  (Menzies 
and  Humphery). 


100  pts.  H2O  dissolve  6.5  pts.  NaoHPO4  + 
12H2O  at  0°;  27.5  pts.  at  30°.  (Tilden,  Chem. 
Soc.  45.  409.) 

Solubility  in  H3PO4+Aq  at  25°. 


In  1000  g.  of  the  solution,  mols. 


Na 

P04 

2.62 
1.56 
2.38 
3.18 
4.65 
5.63 

1.09 
0.78 
1.60 
2.24 
3.55 
3.87 

(D'Ans  and  Schreiner,  Z.  phys.  Ch.  1910,  76. 
101.) 

See  also  above. 

Melts  in  crystal  water  below  100°,  and 
easily  forms  supersaturated  solutions.  (Gay- 
Lussac.) 

Melts  in  crystal  H2O  at  34.6°  (Persoz),  35° 


(Kopp),  40-41°  (Mulder). 

Melts 
Chem.  Soc.  45.  409.) 


in   crystal  H2O   at   35°.      (Tilden, 


Supersaturated  solutions  are  brought  to 
crystallization  by  addition  of  a  crystal  of 
Na2HPO4+12H2O  or  an  isomorphous  sub- 
stance as  NaoHAs04+12H2O.  (Thomson, 
Chem.  Soc.  35.  200.) 

Insol.  in  alcohol. 

Sodium  cfthydrogen  phosphate,  NaH2P04+ 
H2O. 

Very  sol.  in  H2O.  Insol.  in  alcohol. 
(Graham.) 

+2H2O.  Unchanged  on  air.  Very  sol.  in 
H2O,  and  solubility  increases  rapidly  with  the 
temperature.  (Jolv  and  Dufet,  C.  R.  102. 
1391.) 


PHOSPHATE,  SODIUM 


707 


100  pts.  H2O  dissolve  59.9  pts.  at  0°;  84.6 
pts.  at  18°.    (Joly  and  Dufet.) 


+7H,O.    (Salzer,  Arch.  Pharm.  1894,  232. 
365.) 

(Joulie.) 


Solubility  of  NaH2PO4  in  H2O  at  t°. 
G.  of  anydrous  NaH2PO4  in  100  g.  H2O. 
Solid  phase;  NaH2PO4+2H2O. 

Sodium     ort/iophosphate     acid.     NaH2PO4. 
H3P04. 
Hygroscopic.         Decomp.       bv      alcohol. 
(Staudenmaier,  Z.  anorg.  1894,  5/395.) 

Solubility  of  NaH2PO4,  H3PO4  in  H2O  at  t°. 

t° 

G.  NaH2PO4 

"t 

G.  NaH2P04 

0.1 
1.0 
3.0 
5.0 
10.0 
15.0 
20.0 
25.0 
26.0 
27.0 

57.86 

59.08 
61.47 
63.82 
69.87 
76.72 
85.21 
94.63 
96.73 
99.20 

28.0 
30.0 
31.0 
33.0 
34.0 
35.0 
37.0 
40.2 
40.55 

101.71 
106.45 
108.93 
114.31 
117.14 
120.44 
126.76 
138.16 
110.83 

t° 

% 

NaH2P04 
H3P04 

Solid  phase 

-  5.7 
-   7.9 
-11.4 
-38 
-34 
+41 
51.7 
79.7 
85 
101.7 
104.5 
110 
119 
126.5 

20.77 
26.92 
34.15 
56.66 
80.46 
81.82 
83.68 
87.48 
88.65 
91.47 
92.67 
95.79 
97.99 
100 

Ice 

tf 

a 
u 

NaH2PO4 
tt 

(t 
t( 

cc 

"+NaH2P04,  H3PO< 

NaH2P04,  H3P04 
tt 

" 
it 

40  .  8°;  transition  point. 
Solid  phase;  NaH2PO4+H2O. 

41 
42 
45 
50 

142.55 
143.83 
148.20 
158.61 

52 
55 
56 
57 

163.84 
170.85 
173.23 
175.81 

57.4°;  transition  point. 
Solid  phase;  NaH2PO4. 

(Parravano  and  Mieli,  Gazz.  ch.  it.  38,  II. 
536.) 

Solubility  in  anhydrous  H3PO4. 

58 
60 
62 
65 

177.24 
179.33 
181.35 
184.99 

69. 
80. 
90. 
99.1 

190.24 
207.29 
225.31 
246.56 

t 

%  Na.H2P04,  H3P04 

98.5                             52.72 
111                                 69.59 
119                                 77.55 
122                                81.71 
123                                87.20 

(Imadzu,  Chem.  Soc.  1912,  33.  359.) 
Solubility  in  H3P04+Aq  at  25°. 

In  1000  g.  of  the  solution,  mols. 

(Parravano  and  Mieli.) 

-fH2O.    Very  deliquescent.    (Salzer,  Arch. 
Pharm.  1894,  232.  369.) 

Sodium  ps/rophosphate,  Na4P2O7,  and 
+  10H2O. 
Less  sol.   in   H2O  than  sodium  hydrogen 
orthophosphate.    (Clark,  Ed.  J.  Sci.  7.  298.) 
100  pts.  H.O  dissolve  (a)  pts.  Na4P2O7,  (b) 
pts.  Na4P2O7  +  10H2O  at: 
0°        10°      20°         30°         40°         50° 
a.  3.16     3.95       6.23       9.95     13.50     17.45 
b.  5.41     6.81      10.92      18.11     24.97     33.25 

Na 

P04 

6.19 
6.01 
5.12 
4.81 
4.36 
4.06 
4.19 
4.32 
4.65 
4.88 

4.68 
4.67 
4.36 
4.22 
4.08 
4.03 
4.38 
4.96 
5.89 
6.40 

(D'Ans  and  Schreiner,  Z.  phys.  Ch.  1910,  75. 
101.) 

Tnsodium  ^nhydrogen  phosphate. 
Na3H3(P04)2. 

Not  hydroscopic.     Sol.  in  H2O  in  all  pro- 
portions.^   (Joulie,  C.  R.  1902,  134.  604.) 

+l>iH2O.      Sol.    in   H2O.      (Filhol    and 
Senderens,  C.  R.  93.  388.) 


60°  70°  80° 

a.  21.83       25.62        30.04 

b.  44.07        52.11        63.40 

(Poggiale.) 


90°  100° 

35.11        40.26 
77.47        93.11 


Sol.  in  H2feO4.     (Walden,  Z.  anorg.  1902, 
29.  384.) 


708 


PHOSPHATE,  SODIUM  HYDROGEN 


Crystallizes  unchanged  from  NH4Cl+Aq 
(Winkler),  or  cone.  NH4OH+Aq.(Uelsmann.) 

Decomp.  into  orthophosphate  by  heating 
with  H2SO4,  HC1,  HC2H3O2,  or  H3PO4+Aq. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Insol.  in  alcohol.  Insol.  in  methyl  acetate. 
(Naumann,  B.  1909,  42.  3790.) 

Sodium  hydrogen  pyi  ophosphate,  Na2H2P2O7. 

Decomp.  by  H2O.  Sol.  in  H2O  containing 
HC2H3O2  without  decomp.  (Bayer,  J.  pr. 
106.  501.) 

SI.  sol.  in  alcohol.  Much  more  sol.  in  HoO 
than  NaH2PO4. 

+6H2O.  (Rammelsberg,  B.  A.  B.  1883. 
21.) 

100  g.  sat.  solution  contain  14.95  g. 
Na2H2P2O7  at  18°.  (Giran,  A.  ch.  1902,  (7) 
30.  249.) 

NaH3P2O7.  Very  hydroscopic.  (Salzer, 
Arch.-Pharm.  1894,  232.*  369.) 

100  g.  sat.  solution  contain  62.7  g.  at  18°. 
(Giran,  A.  ch.  1902,  (7)  30.  249.) 

Na3HP2O7+H2O.  Sol.  in  3  pts.  H2O. 
(Salzer,  Arch.  Pharm.  1894,  232.  366.) 

+6H2O.  100  g.  sat.  solution  contain  28.17 
g.  Na3HP2O7  at  18°.  (Giran.) 

Sodium  te^raphosphate,  NaeP4O]3. 

Slowly  sol.  in  2  pts.  cold  H2O.  Easily 
decomp. 

+  18H2O.   (Uelsmann.) 

Sodium  hydrogen    fe/raphosphate, 

Na4H2P4013. 
Sol.  in  H2O. 

Sodium  de/caphosphate,  Nai2PioO3i. 

Sol.  in  H2O.  (Fleitmann  and  Henneberg, 
A.  65.  333.) 

Sodium  strontium  diraetaphosphate, 

Na2Sr(P2O6)2+4H2O. 

As  the  NaBa  comp.  (Glatzel,  Dissert. 
1880.) 

Sodium  strontium  ^nraetaphosphate, 

NaSrP3O9+3H2O. 

Easily  sol.  in  H2O  and  acids,  (Fleitmann, 
A.  65.  315.) 

Sodium   strontium  or^ophosphate,  NaSrPO4 

+H20. 

Scarcely  sol.  in  H2O;  sol.  in  acids. 
+9H2O.    (Joly,  C.  R.  104.  905.) 

Sodium  strontium  p^/rophosphate  (?). 

SI.  sol.  in  H2O.  Insol.  in  Na4P2O7+Aq. 
(Baer,  Pogg.  75.  166.) 

Easily  sol.  in  HCl+Aq,  or  HNO8+Aq. 

Sol.  in  NH4OH+Aq. 


Sodium  thallium  p^/rophosphate, 

Na6[Tl(P2O7)2]+6H2O=Na(TlPoO7), 
Na4P2O7+6H2O. 

Decomp.  by  H2O.  (Rosenheim,  B.  1915, 
48.  588.) 

Sodium  thorium  ort/iophosphate, 

NaTh,(P04)*. 

Insol.  in  acids.  (Wallroth,  Bull.  Soc.  (2) 
39.  316.) 

Sodium  thorium  phosphate,  Na2O,  4ThO2, 
3P2O6. 

Insol.  in  HNO3,  HC1,  or  aqua  regia.  (Troost 
and  Ouvrard,  C.  R.  105.  30.) 

5Na2O,  2ThO2,  3P2O5.  Sol.  in  HNO,+Aq. 
(T.  and  O.) 

Na2O,  ThO2,  P2O5.    (T.  and  O.) 

Sodium  thorium  p?/rophosphate,  Na4P2O7, 
ThP2O7+2H2O.' 

(Cleve.) 

Sodium  tin  (stannic)  phosphate,  NaSn2(P04)8. 
(Ouvrard,  C.  R.  111.  177.) 

Na2Sn(PO4)2.    (Wunder,  J.  pr.  (2)  4.  339.) 
6Na2O,  3SnO2,  4P2O5.    (Ouvrard.) 

Sodium  titanium  phosphate,  NaTi2(PO4)3. 
Insol.  in  acids.    (Rose,  J.  B.  1867.  9.) 
6Na2O,  TiO2,  4P2O5.    (Ouvrard,  C.  R.  111. 

177.) 

Sodium  uranium  phosphate,  UO2,Na2O,  P2O5. 
Easily  attacked  bv  acids.     (Colani,  A.  ch. 
1907,  (8)  12.  137.) 

Sodium  uranium  metophosphate,  4UO2,  Na2O, 

3P20&. 
Insol.  in  boiling  HNO3.    (Colani.) 

Sodium  uranium  pyrophosph&te,  3UO2, 

6Na2O,  4P2O6. 
Sol.  in  acids.    (Colani.) 

Sodium  uranyl  phosphate,  Na2O,  UO3,  P2O5. 
(Ouvrard,  C.  R.  110.  1333.) 
2Na2O,  UO3,  P2O5.     (Ouvrard.) 
Na2O,  5UO3,  2P2O5+3H2O.    Insol.  in  H2O; 

decomp.  by  acetic  acid.     (Werther,  A.  68. 

312.) 

Sodium  uran3'l  p^/rophosphate. 

Very  sol.  in  H2O.  (Persoz,  A.  ch.  (3)  20. 
322.) 

Sodium  ytterbium  p?/rophosphate,  NaYbP207. 
Easily  sol.  in  the  strong  acids.    (Wallroth.) 

Sodium  yttrium  p?/rophosphate,  NaYP207. 

Sol.  in  H2O.    (Stromeyer.) 

Insol.  in  H2O.  Easilv  sol.  in  strong  acids. 
(Wallroth.) 


PHOSPHATE,  STRONTIUM  THORIUM 


709 


Sodium  zinc  /nphosphate, 

Na2O,  4ZnO,  3P2O5  +  19H2O. 
Sol.  in  H2O.     (Schwarz,  Z.  anorg.  1895,  9. 
266.) 

Sodium  zinc  tfn'raetaphosphate,  Na2O,  2ZnO, 

3P205. 

Ppt.  Sol.  in  H2O.  (Fleitmann  and  Henne- 
berg,  A.  65.  304.) 

Sodium  zinc  tetrametaphospha.te, 

Na2Zn(PO3)4+6H2O. 
As  K  comp.     (Glatzel,  Dissert.  1880.) 

Sodium   zinc   ocfowetaphosphate, 
Na2Zn3(PO3)8 

Insol.  in  acids. 

Sol.  in  cone.  H2SO4.  (Tammann,  J.  pr. 
1892,  (2)  45.  420.) 

Sodium  zinc  orthophosphate,  NaZnP04. 

Difficultly  sol.  in  H2O  or  acetic  acid.  Easily 
sol.  in  dil.  mineral  acids.  (Scheffer,  A.  145. 
53.) 

2Na2O,  ZnO,  P2O5.  Insol.  in  H2O;  sol.  in 
dil.  acids.  (Ouvrard,  C.  R.  106. 1796.) 

Sodium  zinc  /M/rophosphate,  Na2ZnP2O7. 

Insol.  in  H2O;  sol.  in  dil.  acids.  (Wall- 
roth.) 

3Na4P2O7,  Zn2P2O7+24H2O.  Very  efflores- 
cent. (Pahl.) 

Na4P2O7,  Zn2P2O7+2H  3,  3y2,  and  8H2O. 
Insol.  in  H2O;  sol.  in  Na4P2O7+Aq.  (Pahl, 
Sv.  V.  A.  F.  30,  7.  35.) 

4Na4P2O7,  5Zn2P2O7+20H2O.  Insol.  in 
H2O.  (Pahl.) 

Na4P2O7,  4Zn2P2O7  +  12H2O.  SI.  sol.  in 
H2O.  (Pahl.) 

Sodium  zirconium  phosphate,  Na2O,  4ZrO2, 

3P2O5  =  NaZr2(PO4)3. 

Insol.  in  acids  or  aqua  regia.  (Troost  and 
Ouvrard,  C.  R.  105.  30.) 

6Na2O,  3ZrO2,  4P2O5.  Sol.  in  acids.  (T. 
and  0.) 

4Na2O,  ZrO2,  2P2O6.  Sol.  in  acids.  (T.  and 
O.) 

Sodium  phosphate  fluoride,  Na3PO4,  NaF  + 
12H2O. 

100  pts.  H2O  dissolve,  at  25°,  12  pts.  salt 
and  form  solution  of  1.0329  sp.  gr.;  at  70°, 
57.5  pts.  salt  and  form  solution  of  1.1091  sp. 
gr.  (Briegleb,  A.  97.  95.) 

2Na3PO4,  NaF+19H2O,  and  22  H2O.  Sol. 
in  H2O.  (Baumgarten,  J.  B.  1865.  219.) 

Sodium  phosphate  stannate, 

4Na3PO4,  Na2SnO3+4SH2O. 
(Prandtl,  B.  1907,.  40.  2132.) 


Sodium  phosphate  titanate, 

NazO,  TiO3,  P2O5+3H2O. 
Hygroscopic.      (Mazzuchelli  and  Pantan- 
elli,  C.  C.  1909,  II.  420.) 

Sodium  phosphate  vanadate. 
See  Phosphovanadate,  sodium. 

Strontium  wonoraetaphosphate,  Sr(PO3)2. 

Insol.  in  H2O  and  acids.  Not  decomp.  by 
alkali  carbonates +Aq.  (Maddrell,  A.  61.  61.) 

Strontium  hexametaphosph&te. 

Nearly  insol.  in  H2O;  easily  sol.  in  acids. 
(Ludert,  Z.  anorg.  5.  15.) 

Strontium    or^ophosphate,   basic,    Sr(OH)2, 

Sr3(PO4)2. 
(Woyczynski,  Z.  anorg.  1894,  6.  311.) 

Strontium  or/Aophosphate,  Sr3(PO4)2. 

Insol.  in  H2O.  Sol.  in  HCl+Aq.  (Erlen- 
meyer,  J.  B.  1857.  145.) 

Strontium  hydrogen  phosphate,  SrHPO4. 
Insol.  in  H2O.     Sol.  in  H3PO4,  HC1,   or 

HNO3-|-Aq.      (Vauquelin.)      Easily    sol.    in 

cold   ammonium   nitrate,    chloride,    or   suc- 

cinate+Aq,  but  is  partly  precipitated  by  a 

little  NH4OH+Aq.    (Brett.) 

Sol.  in  boiling  NH4Cl+Aq.    (Fuchs,  1834.) 

Sol.  in  Na  citrate +Aq.     (Spiller.) 

Partly  decomp.  by  boiling  Na2CO3,   and 

K2CO3+Aq.     (Dulong.) 

SrH4(PO4)2+2H2O.     Decomp.  by  treating 

with  H2O,  leaving  4.29%SrHPO4.     (Barthe.) 

Strontium    phosphate,    acid,    H->O,    2SrO, 

3P2O5+zH2O. 

Entirely  sol.  in  H2O.  (Barthe,  C.  R.  114. 
1267.) 

Strontium   p^/rophosphate,   Sr2P2O7-fH2O. 

Somewhat  sol.  in  H2O.  Easily  sol.  in  HC1 
or  HNO3+Aq.  Insol.  in  HC2H3O2  or 
Na4P2O7-|-Aq.  (Schwarzenberg,  A.  65.  144.) 

+2}/6H,O.  (Knorre  and  Oppelt,  B.  21. 
773.) 

Strontium    hydrogen    pyrophosphsite, 

SrH2P2O7,  2Sr,P2O7+6H2O. 
Ppt.    (Knorre  and  Oppelt,  B.  21.  772.) 
SrH2P2O7,    3Sr2P2O7+H2O,    and    +2H2O. 

(Knorre  and  Oppelt.) 
Sr9H2(P2O7)6+8H2O,  and  +12H2O. 
Ppt.     (Pahl,  Gm.  -  K.  2,  2.  172.) 
Sr19H2(PoO7)10+5H2O,  +18H2O    and 

+20H2O. 
Insol.  in  Sr(NO3)2+Aq  or  Na4P2O7+Aq. 

(Pahl,  Gm.-K.  2,  2.  171.) 

Strontium  thorium   phosphate, 

Th2O.  SrO,  P2O5. 
(Colani,  C.  R.  1909,  149.  209.) 


710 


PHOSPHATE,  STRONTIUM  URANIUM 


Strontium  uranium  raetaphosphate, 

UO2,  SrO,  P2O5. 
(Colani,    A.    ch.    1907,  (8)  12.  141.) 

Strontium  uranyl  phosphate, 

SrO,  4UO3,  2P2O5+21H2O. 

(Blinkoff,  Dissert.  1900.) 

2SrO,  5UO3,  2P2O6+24H2O.    As  Ba  comp. 
(Blinkoff.) 

Strontium    phosphate    chloride,    3Sr3(PO4)2, 


Strontium  apatite.  Insol.  in  H2O.  (De- 
ville  and  Caron.) 

Tellurium  phosphate  (?). 
Insol.  in  H2O.     (Berzelius.) 

Thallous  wetaphosphate,  T1PO3. 
Two  modifications: 
a.  Difficultly  sol.  in  H2O. 
j8.  Extremely  easily  sol.  in  H2O.     (Lamy.) 

Thallous  ort/bphosphate,  T13PO4. 

1  pt.  is  sol.  in  201.2  pts.  H2O  at  15°,  and  149 
pts.  boiling  H2O;  sol.  in  HNO3+Aq. 
(Crookes.)  SI.  sol.  in  HC2H3O2+Aq.  Very 
easily  sol.  in  solutions  of  NH4  salts.  (Car- 
stanjen.)  Insol.  in  alcohol.  (Lamy.) 

Thallous  hydrogen  phosphate,  T12HPO4. 

Anhydrous.  Much  less  sol.  in  H2O  than 
the  hydrous  salt,  but  easily  sol.  in  a  solution 
of  the  hydrous  salt.  (Lamy.) 

+  ^H2O.  Easily  sol.  in  H2O.  Insol.  in 
alcohol.  (Lamy.) 

Composition  is  HT12PO4,  2H,T1PO4. 
(Rammelsberg,  W.  Ann.  16.  694.) 

Thallous    cfthydrogen    phosphate,    T1H2PO4. 
Verv  easily  sol.  in  H2O.    Insol.  in  alcohol. 
(Rammelsberg,  B.  3.  278.) 

Tnthallous  tfnhydrogen  phosphate,  T12HPO4. 
2T1H2PO4. 

True  composition  of  T12HPO4  of  Lamy. 
(Rammelsberg.) 

Thallous  pyrophosphate,  T14P2O7. 

Sol.  in  2.5  pts.  H2O  with  slight  decomposi- 
tion. (Lamy.) 

+2H2O.  More  sol.  in  H2O  than  the  above 
salt,  with  partial  decomp.  (Lamy.) 

Thallous  hydrogen  pyrophosphate,  H2T12P2O7 

+H2O. 
Very  sol.  in  H2O.    (Lamy.) 

Thallic    phosphate,    basic,    2T12O3,    P2O6  + 

5H2O. 
Insol.  in  H2O. 


ThaUic  phosphate,  basic,  T18P9O27  +  13H2O. 
(Rammelsberg,  W.  Ann.  16.  694.) 
T1,;P4019+12H20.     (R.) 

Thallic  phosphate,  T1PO4+2H2O. 

Completely  insol.  in  H2O.  Sol.  in  cone. 
HNO8,  and  dil.  HCl+Aq.  (Willm.) 

Thorium  metophosphate,  Th(PO3)4. 

Insol.  in  H2O.    (Troost,  C.  R.  101.  210.) 

Thorium  wetaphosphate,  ThO2,  2P2O5. 
Insol.  in  acids.     (Johnsson,  B.  22.  976.) 

Thorium   ort/wphosphate,  Th3(PO4)4+4H2O. 

Insol.  in  H2O  and  phosphoric  acid  (Ber- 
zelius); also  acetic  acid.  (Cleve.) 

Sol.  in  HC1,  and  HNO3+Aq.     (Cleve.) 

Thorium  hydrogen  phosphate,  ThH2(PO4)o-f 

H20. 
Precipitate. 

Thorium   pi/rophosphate,   ThP2O7+2H2O. 

Precipitate.  Insol.  in  H2O.  Sol.  in  great 
excess  of  pyrophosphoric  acid  or  sodium  pyro- 
phosphate+Aq.  (Cleve.) 

Thorium  phosphate  bromide. 
See  Bromophosphate,  thorium. 

Thorium  phosphate  chlroide. 
See  Chlorophosphate,  thorium. 

Tin   (stannous)    phosphate,   5SnO,   4P2O5+ 

4H2O. 

Insol.  in  H2O.    (Lenssen,  A.  114.  113.) 
Sn3(PO,f)2.    Insol.  in  H«O.    Sol.  in  mineral 

acids.     (Kiihn.) 

Insol.  in  NH4C1  or  NH4NO3+Aq.    Sol.  in 

KOH+Aq. 

Tin  (stannic)  phosphate,  2SnO2,  P2Oc-f 
10H20. 

Insol.  in  H2O  or  HNO3  +  Aq.  (Reynoso,  J. 
pr.  54.  261.) 

Anhydrous.  Insol.  in  acids.  (Hautefeuille 
and  Margottet,  C.  R.  102.  1017.) 

Tin  (stannic)  phosphate,  SnP2O7. 

Insol.  in  acids.  (Hautefeuille  and  Margot- 
tet, C.  R.  102.  1017.) 

Tin    (stannous)    phosphate    chloride,    3SnO, 

P205,  SnCla+HW). 

Not  decomp.  by  hot  H2O.  (Lenssen,  A. 
114.  113.) 

Titanium  phosphate,  Ti2PA>  =  2TiO2,  P2O6. 

Insol.  in  acids.  (Hautefeuille  and  Margot- 
tet, C.  R.  102.  1017.) 

(Ouvrard,  C.  R.  111.  177.) 

+3H2O.     Ppt.     Insol.   in  H2O.     (Merz.) 


PHOSPHATE,  YTTRIUM 


711 


TiOa,  P2O6.  (Knop.)  Is  NaTi2(PO4)3. 
(Wunder,  J.  B.  1871.  324.) 

H8TiP07.    Sol.  in  HC1,  HNO8,  H2S04. 

SI.  sol.  in  H3PO4. 

Sol.  in  KOH,  NH4OH,  (NH4)2CO3  and 
(NH4)2HP04+Aq. 

Very  si.  sol.  in  acetic  acid.  (Faber,  Z. 
anal.  1907,  46.  288.) 

Uranous  wetaphosphate,  U(PO3)4. 

Insol.  in  HNO3,  HC1,  or  H2SO4,  even 
when  hot  and  cone.  (Colani,  A.  ch.  1907,  (8) 
12.  105.) 

Uranic  raetophosphate,  U2(PO3)c. 

Insol.  in  H2O  and  acids.  (Plautefeuille  and 
Margottet,  C.  R.  96.  849.) 

Uranous  or^ophosphate,  U3(PO4)4. 

More  easily  attacked  by  acids  than  the  pyro 
and  meta  phosphates,  especially  by  HNO3. 
(Colani,  A.  ch.  1907,  (8)  12.  123.) 

Uranous  hydrogen  ortAophosphate,  tJHPO4+ 

H2O. 

Insol.  in  H2O.  Insol.  in  dil.,  si.  sol.  in 
cone.  HCl+Aq.  Decomp.  by  KOH+Aq, 
not  by  NH4OH+Aq.  (Rammelsberg,  Pogg. 
59.  1.) 

Uranous  p?/r0phosphate,  UP2O7. 
Insol.  in  H2O. 
SI.  sol.  in  min.  acids.    (Colani.) 

Uranous  phosphate,  2U02,  P2O5. 

Easily  attacked  by  boiling  HNO3. 
(Colani.) 

UO2,  P2O6+5H2O.  Insol.  in  H2S04  and 
in  HCl+Aq  of  medium  concentration.  Sol. 
in  very  cone.  HCl+Aq.  (Aloy,  Dissert. 
1901.) 

Uranyl  wetaphosphate,  UO2(PO3)2. 
(Rammelsberg,  B.  A.  B.  1872.  447.) 
UO3,  2P2O5.     Insol.  in  acids.     (Johnsson, 

B.  22.  976.) 

Uranyl  or^ophosphate,  UO2HPO4+1^H2O. 

Insol.  in  H2O. 

+3HoO. 

+4H2"0. 

+4V£H2O.  Insol.  in  H,O.  Sol.  in  67,000 
pts.  HC2H3O2+Aq,  50,000  pts.  NH4C2H3O2  + 
Aq,  and  300,000  pts.  of  a  mixture  of  the  above 
two  solutions.  Sol.  in  K2CO3  or  Na2CO3  + 
Aq.  (Kitschin,  C.  N.  27.  199.) 

Uranyl  cfthydrogen  phosphate, 

UO2H4(PO4)2+3H20. 

Decomp.  by  H2O.  Sol.  in  H3PO4+Aq. 
(Werther,J.pr.43.322.) 


Uranyl  p^/rophosphate,  (UO2)2P2O7+5H2O. 

Efflorescent.  Insol.  in  H2O.  Sol.  in 
HNOs+Aq,  and  Na4P2O7+Aq.  Insol.  in 
Na2HPO4+Aq.  Insol.  in  alcohol  or  ether. 
(Girard,  C.  R.  34.  22.) 

+4H2O.     (Casteing,  Bull.  Soc.  (2)  34.  20.) 

Uranyl  tetraphosphate  (?),  UO2P4On. 
(Johnsson,  B.  22.  978.) 

Uranous  ortftophosphate   chloride,  U3(PO4)4, 

UC14. 

SI.  sol.  in  HCl+Aq.  Sol.  in  HNO3  and 
HNOs+HCl.  (Colani,  A.  ch.  1907,  (8)  12. 

127.) 

Uranous  hydrogen   or^ophosphate  chloride, 

U(HPO4)2,  UC14. 
Very  si.  sol.  in  H2O.    (Aloy,  Dissert.  1901.) 

Vanadium  phosphate,  (VO2)H2PO4+4^H2O. 
Sol.  in  H2O. 
See  Phosphovanadic  acid. 

Vanadium  pi/rophosphate, 

V4(P2O7)3+30H2O. 

Insol.  in  H2O.     (Rosenheim,  B.  1915,  48. 
590.) 

Divanadyl  phosphate. 

Very  deliquescent,  and  sol.  in  H2O.  Insol. 
in  alcohol.  (Berzelius.) 

Ytterbium  wetophosphate,  Yb(PO3)3. 

Insol.  in  H,O.  (Cleve,  Z.  anorg.  1902,  32. 
149.) 

Ytterbium  ortfiophosphate,  YbPO4+43/£H2O. 
Ppt.    (Cleve.) 

Ytterbium  phosphate,  Yb2O3,  2P2O5+5H2O. 
Sol.  in  H2O.     (Cleve.) 

Yttrium  wetophosphate,  Y(PO3)3. 
Insol.  in  H2O  or  acids.    (Cleve.) 

Yttrium  ortftophosphate,  YPO4. 

Anhydrous.  Insol.  in  H2O  or  acids  after 
ignition. 

Min.  Xenotime.  Insol.  in  cone,  acids.  SI. 
sol.  in  much  cone.  HCl+Aq,  but  easity  sol. 
therein  when  first  heated  with  a  little  HC1+ 
Aq.  (Wartha,  A.  139.  237.) 

Yttrium  hydrogen  or^ophosphate,  Y2(HPO4)3. 
Decomp.  by  boiling  with  H2O  into  insol. 
YPO4  and  sol.  acid  salt. 

Yttrium  p?/rophosphate,  YHP2O7+3KH2O. 

Difficultly  sol.  in  acids.  Decomp.  by 
H2SO4.  Sol.  in  Na4P2O7+Aq.  (Cleve.) 

2Y2O3,  3P2Oft.  Insol.  in  acids.  (Johnsson, 
B.  22.  976.) 


712 


PHOSPHATE,  ZINC 


Zinc  raetaphosphate. 

Sol.  in  H2O.    (Berzelius.) 

Zinc  cftwetaphosphate,  ZnP2O6. 

Sol.  only  in  boiling  H2SO4.  (Fleitmann, 
Pogg.  78.  350.) 

Not  decomp.  by  boiling  Na2S  or  (NH4)2S  + 
Aq. 

+4H2O.  Insol.  in  H2O,  but  decomp.  by 
boiling  therewith.  (Fleitmann,  Pogg.  78. 
25S.) 

Sol.  in  4  pts.  H2O.  Cone.  H2SO4  decomp. 
it  easily;  other  acids  act  slightly.  (Glatzel, 
Dissert.  1880.) 

Difficultly  decomp.  by  boiling  acids. 

Zinc  Znmetaphosphate,  Zn3(PO3)6-h  9H2O. 

1  1.  H2O  dissolves  0.1  g.  at  20C.  (Tam- 
mann,  J.  pr.  1892,  (2)  45.  426.) 

Zinc  tetrametaphosphate,  Zn2(PO3)4  +  10H2O. 

Sol.  in  55  pts.  H2O.  Decomp.  by  acids 
only  on  boiling.  (Glatzel,  Dissert.  1880.) 

Somewhat  sol.  in  HNO3+Aq.  Sol.  in 
boiling  H2SO4.  (Glatzel.) 

Zinc  or^ophosphate,  Zn3(PO4)2+4H2O. 
Insol.  in  H2O.    Easily  sol.  in  acids,  NH4OH, 

(NH4)2CO3,    (NH4)2SO4,    or    NH4NO3+Aq. 

(Heintz,  A.  143.  356.) 
Sol.  in  NH4Cl+Aq.    (Fuchs.) 
Easily  sol.  in  Zn  salts +Aq.    (Rose.) 
Insol.  in  liquid  NH3.     (Franklin,  Am.  Ch. 

J.  1898,  20.  830.) 
Min.  Hopeite. 
+6H2O.    (Reynoso.) 

Zinc  hydrogen  phosphate,  ZnHPO4+H2O. 

Insol.  in  H2O;  sol.  in  H3PO4+Aq.  (Gra- 
ham.) 

Zinc  tetrohydrogen  phosphate,  ZnH4(PO4)2  + 

2H2O. 

Nearly  insol.  in  H«O,  but  decomp.  thereby 
into  HSPO4  and  lOZnO,  4P2O5  +  10H2O. 
(Demel,  B.  12.  1171.) 

Zinc  phosphate,  lOZnO,  4P2O5  +  10H2O. 
Insol.  in  H2O.    (Demel,  B.  12.  1171.) 

Zinc  pyrophosphate,  Zn2P2O7+3/2H2O. 

Ppt.  Sol.  in  H2SO3+Aq.  Sol.  in  acids, 
KOH+Aq,  NH4OH+Aq.  (Schwarzenberg, 
A.  65.  151.) 

Sol.  in  Na4P2O7+Aq  (Gladstone),  and  in 
ZnSO4+Aq.  (Rose.) 

Insol.  in  acetic  acid.  (Knorre,  Z.  anorg. 
1900,  24.  389.) 

+5H2O.  Insol.  in  H2O.  (Pahl,  J.  B.  1873. 
229.) 

Zinc  hydrogen  pyrophosphate. 

Sol.  in  H2O.    (Pahl,  Sv.  V.  A.  F.  30,  7.  45.) 


Zinc  raetaphosphate  ammonia. 
Ppt.    (Bette.) 

Zinc  or^ophosphate  ammonia,  2ZnO,  P2O5, 
3NH3+8H2O. 

(Rother,  A.  143.  356.) 

6ZnO,  3P2O6,  8NH3+4H2O.  (Schweikert, 
A.  145.  517.) 

Zinc    pyroohosphate     ammonia,     3Zn2P2O7, 

4NH3+9H2O. 
Ppt.    Insol.  in  H2O.    (Bette.) 

Zirconium  oriAophosphate,  5ZrO2,  4P2O5  + 
8H2O. 

Somewhat  sol.  in  acids.  (Hermann,  J.  pr. 
97.  321.) 

Insol.  in  acids.  (Paykull,  Bull.  Soc.  (2)  20. 
65.) 

2ZrO2,  P2O5.  Not  attacked  by  acids. 
(Hautefeuille  and  Margottet,  C.  R.  102. 
1017.) 

Zirconiuni  pyrophosphate,  Zr(PO3)2. 
(Knop,  A.  159.  36.) 

Phosphoricovanadicotungstic  acid. 

Ammonium  phosphoricovanadicotungstate, 
14(NH4)2O,    2P->O3,     7V2O3,     31WO3+ 
78H2O. 
Sol.  in  H2O.     Insol.  in  alcohol,  ether,  CS2 

and  benzene.     (Rogers,  J.  Am.  Chem.  Soc. 

1903,  25.  305.) 

Phosphorimidamide,  PN2H3. 
(Joannis,  C.  R.  1904,  139.  365.) 

Phosphorimide,  P2(NH)3. 

Very  sol.  in  ammoniacal  solution  of  NHJ. 
(Hug6t,  C.  R.  1905,  141.  1236.) 

Phosphornitryl,  PON. 
See  Phosphoryl  nitride. 

Phosphorosomolybdic  acid,  P2O3, 

24MoO3+63H2O. 

(Rosenheim  and  Pinsker,  Z.  anorg.  1911, 
70.  77.) 

Ammonium  phosphorosomolybdate, 

2(NH4)2O,  2H3PO3,  12Mo 
Insol.  in  cold,   slightly  sol.  in  hot  H2O. 
(Gibbs,  Am.  Ch.  J.  5.  361.) 

Phosphorosophosphomolybdic  acid. 

Ammonium     phosphorosophosphomolybdate, 
9(NH4)2O,    2H3PO3,    3P2O5,    72MoO3  + 
38H2O. 
Nearly  insol.  in  H2O.    (Gibbs.) 


PHOSPHITE,  COBALTOUS 


713 


Phosphorosophosphotungstic  acid. 

Potassium  phosphorosophosphotungstate, 

5K2O,  2H3PO3,  P2Oft,  24WO3  +  13H2O. 
Sol.  in  much  boiling  H2O.    (Gibbs,  Am.  Ch. 
J.  7.  313.) 

Phosphorosotungstic  acid. 

Ammonium  phosphorosotungstate,  6(NH4)2O, 

4H»PO8,  22WO3+25H2O. 
SI.  sol.  in  cold  H20. 

Potassium  ,  5K2O,  16H3PO3,  32WO3  + 

46H20. 
SI.  sol,  in  hot  H2O. 

Sodium    ,    2Na2O,    8H3PO3,    22WO3  + 

35H2O. 

Nearly  insol.  in  cold,  si.  sol.  in  hot  H2O. 
(Gibbs,  Am.  Ch.  J.  7.  313.) 

Phosphorous  anhydride,  P2O3. 
See  Phosphorus  ^n'oxide. 

Phosphorous  acid,  H3PO3. 

Deliquescent.    Very  sol.  in  H2O. 

Phosphites. 

The  neutral  alkali  phosphites  are  sol.  in 
H2O;  most  of  the  others  are  si.  sol.  in  H2O, 
but  sol.  in  H3PO3+Aq;  all  are  insol.  in 
alcohol. 

Aluminum     phosphite,     basic.     A12(HPO3)3. 

A12(OH)6. 

Ppt.  (Griitzner,  Arch.  Pharm.  1897,  235. 
698.  j 

Aluminum  phosphite. 

Precipitate. .  (Rose,  Pogg.  9.  39.) 
SI.  sol.  in  H2O. 

Ammonium  phosphite,  (NH4)2HPO3+H2O. 

Very  deliquescent,  and  sol.  in  H2O.  (Rose, 
Pogg.  9.  28.) 

Sol.  in  2  pts.  cold,  and  less  hot  H2O.  Insol. 
in  alcohol.  (Berzelius.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4328.) 

Ammonium  hydrogen  phosphite, 

(NH4H)HPO3. 

Very  deliquescent,  and  sol.  in  H2O.  1  pt. 
H2O  dissolves  1.71  pts.  salt  at  0°;  1.9  pts.  at 
14.5°;  and  2.60  pts.  at  31°.  (Amat,  C.  R. 
105.  809.) 

Ammonium  hydroxylamine  phosphite, 

NH4(NH3OH)HPO3. 

Sol.  in  H2O  and  abs.  alcohol.  (Hofmann, 
Z.  anorg.  1898,  16.  466.) 


Ammonium  magnesium  phosphite, 
(NH4)2Mg3(PH03)4  +  16H20. 
Slightly  sol.  in  H2O.    (Rammelsberg,  Pogg. 
131.  367.) 

Antimonyl  phosphite,  (SbO)H2PO3. 

Very  sol.  in  H2O  containing  HG1.  (Griitz- 
ner, Arch.  Pharm.  1897,  235.  694.) 

Barium  phosphite,  BaHPO3. 

100  pts.  H2O  dissolve  0.25  pt.    (lire.) 

Very  slightly  sol.  in  H2O,  and  decomp.  by 
boiling  H2O.  (Dulong.) 

Easily  sol.  in  H2O  containing  NH4C1. 
(Wackenroder,  A.  41.  315.) 

Sol.  in  H3PO3  +  Aq  or  HC1  +  Aq.    (Railton.) 

Barium  hydrogen  phosphite,  Ba2H2(HPO3)3  + 

8PI2O. 

Easily  sol.  in  H2O,  but  decomp.  by  boiling 
therewith.  Insol.  in  alcohol.  (Rammelsberg, 
Pogg.  132.  496.) 

Barium  dihydrogen  phosphite,  BaH2(HPO3)2 


Easily  sol.  in  H2O.    (Rose,  Pogg.  9.  215.) 

+H2O.  Sol.  in  H2O;  decomp.  by  boiling 
H2O  into  a  neutral  insol.,  and  an  acid  sol.  salt. 
(Wurtz,  A.  58.  66.) 

+2H2O.  Easily  sol.  in  H2O.  (Rammels- 
berg, Pogg.  132.  496.) 

Insol.  in  alcohol.    (Wurtz.) 

Bismuth  phosphite,  2Bi2O3,  3P2O3. 

Insol.  in  H2O. 

Bi2(HPO3)3+3H2O.  Ppt.  (Griitzner, 
Arch.  Pharm.  1897,  235.  696.) 

Decomp.  by  H2S.  Not  decomp.  by  KOH 
+Aq.  (Vanino,  J.  pr.  1906,  (2)  74.  151.) 

Cadmium  phosphite,  CdHPO3+3H2O. 
Ppt.    (Rose,  Pogg.  9.  41.) 

Calcium  phosphite,  CaHPO3+3/2H2O. 

SI.  sol.  in  H2O;  the  aqueous  solution  is  de- 
comp. by  boiling. 

+H2O.  Sol.  in  NH4Cl+Aq.  (Wacken- 
roder, A.  41.  315.) 

Insol.  in  alcohol. 

Calcium  hydrogen  phosphite,  CaH2(HPO3)2  + 

H2O. 

Sol.  in  H2O.  Aqueous  solution  is  decomp. 
by  alcohol.  (Wurtz,  A.  ch.  (3)  7.  212.) 

Chromic  phosphite. 

Precipitate.  Almost  insol.  in  H2O.  (Rose, 
Pogg.  9.  40.) 

Cobaltous  phosphite,  CoPHO3+2H2O. 
Ppt.    SI.  sol.  in  H2O.    (Rose.) 


714 


PHOSPHITE,  CUPRIC 


Cupric  phosphite,  CuHPO3+2H2O. 

Ppt.  Insol.  in  H2O.  (Wurtz,  A.  ch.  (3) 
16.  213.) 

Didymium  phosphite,  Di2(HPO3)3. 

Precipitate.  (Frerichs  and  Smith,  A.  191. 
331.) 

Glucinum  phosphite. 

Precipitate.  Insol.  in  H2O.  (Rose,  Pogg. 
9.  39.) 

Iron  (ferrous)  phosphite,  FeHPO3+a;H2O. 

Ppt.  Nearly  insol.  in  H2O.  (Rose,  Pogg. 
9.  35.) 

Iron   (ferric)   phosphite,  basic,   Fe2(HPO3)3, 

Fe2(OH)6. 

(Griitzner,  Arch.  Pharm.  1897,  235.  697.) 
Fe4(HPO3)6,      Fe(OH)3+5H2O.       Hydro- 

scopic.    (Berger,  C.  R.  1904,  138.  1500.) 

Iron  (ferric)  phosphite,  Fe2(HPO3)2+9H2O. 
Ppt.    Sol.  in  iron  alum+Aq.     (Rose.) 

Lanthanum  phosphite,  La2(HPO3)3. 
Precipitate.    (Smith.) 

Lead  phosphite,  basic,  4PbO,  P2O3+2H2O. 
.  Ppt.    (Rose,  Pogg.  9.  222.) 

3PbO,  F2O,+HS6.  Insol.  in  H2O.  Sol.  in 
warm  dil.  H3PO3-|-Aq,  from  which  it  is 
pptd.  by  NH4OH+Aq.  (Wurtz,  A.  ch.  (3) 
16.  214.) 

Lead  phosphite,  PbHPO3, 

Insol.  in  H2O.  Very  si.  sol.  in  a  solution 
of  phosphorous  acid;  easily  sol.  in  cold  HNO3 
+Aq.  (Wurtz.) 

Lead  hydrogen  phosphite,  PbH4(PO3)2' 
Decomp.  by  H2O.    (Amat,  C.  R.  110.  901.) 

Lead  pyrophosphite,  PbH2P2O5. 

Gradually  decomp.  by  H2O  into  H3PO3  and 
PbHPO3.  (Amat,  C.  R.  110.  903.) 

Lithium  hydrogen  phosphite,  LiH2PO3. 

Very  sol.  in  H2O.  (Amat,  A.  ch.  (6)  24. 
309.) 

Lithium  p^/rophosphite,  Li2H.,P2O5. 

Very  sol.  in  H,O.  (Amat.  A.  oh.  1891,  (6) 
24.  352.) 

Magnesium   phosphite,    MgHPO3+3H2O. 
SI.  sol.  in  H2O.     (Rose,  Pogg.  9.  28.) 
Sol.  in  400  pts.  H2O.    (Berzelius.) 
+4H,0. 

Magnesium    pyrophosphite,    Mg(H2PO3)2. 

Very  sol.  in  H2O.  (Amat.  A.  ch.  1891,  (6) 
24.  313.) 


Manganous  phosphite, 

Difficultly  sol.  in  H2O,  easily  in  MnCl2  or 
MnSO4+Aq.-  (Rose,  Pogg.  9.  33.) 

Nickel  phosphite,  NiHPO3+3MH2O. 
Ppt.    SI.  sol.  in  H2O. 

Potassium  phosphite,  K2HPO3. 

Very  deliquescent.  Very  sol.  in  H2O. 
Insol.  'in  alcohol.  (Dulong'.) 

Potassium  hydrogen  phosphite,  (KH)HPO3. 

1  pt.  H2O  dissolves  about  1.72  pts.  salt  at 
20°.  (Arnat.  C.  R.  106.  1351.) 

K2HPO3,  2H3PO3.  Very  sol.  in  H2O. 
(Wurtz,  A.  58.  63.) 

Sol.  in  3  pts.  cold,  and  in  less  hot  H2O. 
(Fourcroy  and  Vauquelin.) 

Potassium   pyrophosphite,    K2H.,P2O5. 

Very  sol.  in  H2O.  (Amat.  A,  ch.  (6)  24. 
351.) 

Sodium  phosphite,  basic,  Na2HPO3, 
NaOH  (?). 

Not  obtained  in  pure  state  (Zimmerman, 
B.  7.  290);=Na8PO«  (Wislicenus.) 

Does  not  exist.    (Amat.) 

Sodium   phosphite,   Na2HPO3+5H,O. 

Deliquescent,  and  very  sol.  in  H20.  In- 
sol. in  alcohol. 

Correct  formula  for  Na3PO3  of  Rose  and 
Dulong. 

Sodium  hydrogen  phosphite.  (NaH)HPO3-f 


0.56  pt.  salt  dissolves  in  1  pt.  H2O  at  0°; 
0.66  pt.  at  10°;  1.93  pts.  at  42.°  (Amat, 
C.  R.  106.  1351  j 

Na2H4(HPO3)3+H2O.  Deliquescent  in 
moist  air.  Sol.  in  2  pts.  cold,  and  about  the 
same  amt.  hot  H2O.  SI.  sol.  in  spirit.  (Four- 
croy and  Vauquelin.) 

Sodium  pyrophosphite,  Na2H2P2O5. 

Very  sol.  in  H2O  with  gradual  decomp.  into 
Na2HPO3.  (Amat.) 


Strontium    phosphite,    SrHPOa  +  l 

Difficultly  sol.  in  H2O.  Aqueous  solution 
decomp.  on  heating  into  a  sol.  acid  salt  and 
an  insol.  basic  salt. 

Strontium  hydrogen  phosphite,  SrH4(PO3)2. 
Very  sol.  in  H2O.  (Amat,  A.  ch.  (6)  24.  312.) 

Thallous  hydrogen  phosphite,  T1H2PO3. 
Very  sol.  in  H2O.  (Amat,  A.  ch.  (6)  24.  310.) 

Thallous  pyrophosphite,  T12H2P2O5. 

Deliquescent.    Very  sol.  in  H2O.     (Amat.) 


PHOSPHORUS 


715 


Tin  (stannous)  phosphite,  SnHPO3. 

Ppt.  Sol.  in  HCl+Aq.  (Rose,  Pogg.  9 
45.) 

Tin  (stannic)  phosphite,  2SnO2,  P2O3. 
Ppt.     (Rose,  Pogg.  9.  47.) 

Titanium  phosphite  (?) 

Precipitate.     (Rose,  Pogg.  9.  47.) 

Uranyl  phosphite,  (UO2)3H2(HPO3)4  +  12H2O 
Precipitate.      (Rammelsberg.    Pogg.    132, 
500.) 

Zinc  phosphite,  ZnHPO3. 

Sol.  in  H2O.  (Rammelsberg,  Pogg.  132. 
481.) 

+2;HjH2O.  More  easily  sol.  in  cold  than 
warm  H2O.  (Rammelsberg.) 

Zinc  phosphite,  acid,  Zn2H3P3O8. 

Sol.  in  H2O. 

+2H2O.  Sol.  in  HoQ.  (Rammelsberg, 
Pogg.  132.  498.) 

Zn3H5P5O13.     Sol.  in  H2O. 

+3H2O.     Sol.   in   H2O.      (Rammelsberg.) 

Zn2H9P5OJ4.    Sol.  in  H2O. 

-fH2O.      Sol.    in    H2O.      (Rammelsberg.) 

Zirconium  phosphite,  Zr(PO3)->+H2O. 

Ppt.  Nearly  insol.  in  dil.  mineral  acids. 
(Hauser,  Z.  anorg.  1913,  84.  92.) 

Phosphorous  anhydride,  P2O3. 
See  Phosphorus  ^noxide. 

Phosphorus,  P. 

(a)  Ordinary  white  phosphorus.  Insol.  in 
H2O,  but  slowly  decomp.  thereby  (G.  K.); 
very  si.  sol.  in  H2O.  (Berzelius  and  others.) 

A  pure  aqueous  solution  containing  0.1  g. 
P  in  500  cc.  H2O  can  be  obtained  by  dissolv- 
ing 0.1  g.  P  in  CS2  mixed  with  ether  and  hot 
alcohol;  this  solution  is  poured  into  500  cc. 
boiling  H2O  free  from  air,  and  the  boiling 
continued  with  stirring  until  the  alcohol,  ether 
and  CS2  are  boiled  off.  (Bokorny,  Ch  Ztg 
1896,  20.  1022.) 

100  g.  H2O  sat.  with  P  contains  0.0003  g 
P.  (Stich,  C.  C.  1903, 1.  1291.) 

Sol.  with  decomp.  in  hot  cone.  HNO3+Aq. 

Decomp.  by  boiling  caustic  alkalies +Aq 

Easily  sol.  in  SC12,  especially  if  hot.  (Woh- 
ler.) 

Sol.  in  sulphur  phosphides. 

Largely  sol.  in  PC13. 

Easily  sol.  in  PC16. 

Sol.  in  PBr3.  Sol.  in  PSC13,  easily  on  warm- 
ing, separating  on  cooling.  •  (Serullas,  A 
ch.  1829,  42.  25.) 

Sol.  in  liquid  SO2.  (Sestini,  Bull  Soc 
1868,  (2)  10.  226.) 

Sol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 


Sol.  in  S2C12  without  foaming.  (Nicolardot, 
C.  R.  1908,  147.  1304.) 

Sol.  in  PS4C15.  (Gladstone,  A.  1850,  74. 
91.) 

Sol.  in  320  pts.  cold  alcohol  of  0.799  sp.  gr., 
and  in  240  pts.  of  the  same  when  warm. 
Pptd.  from  alcoholic  solution  by  H2O.  (Biich- 
ner.) 

One  grain  P  dissolves  in  1  ounce  abs.  alco- 
hol. (Schacht.) 

Sol.  in  20  pts.  absolute  ether  at  20°  and 
240  pts:  ordinary  ether  at  20°.  (Bucholz.) 

Sol.  in  80  pts.  absolute  ether  at  15.5°,  and 
240  pts.  ordinary  ether  at  15.5°.  (Brug- 
natelli,  A.  ch.  24.  73.) 


Solubility  of  P4  in  100  g.  ether  at  t°. 


t° 

G.  phosphorus 

Sp.  gr. 

0 

0.4335 

5 

0.62 

8 

0.79 

' 

10 

0.85 

15 

0.9 

at  13°  0.7257 

18 

1.005 

20 

1.04 

at  19°0.7i87 

23 

1.121 

25 

1.39 

0.7283 

28 

1.601 

30 

1.75 

33 

1.8 

35 

1  .  9984 

(Christomanos,  Z.  anorg.  1905,  46.  136.) 


Solubility  of  P4  in  100  g.  benzene  at  t°. 


t° 

G.  phosphorus 

Sp.  gr. 

0 

1.513 

5 

1.99 

8 

2.31 

10 

2.4 

15 

2.7 

at  13°  0.8959 

18 

3.1 

20 

3.21 

at  19°  0.8912 

23 

3.3995 

at  22°  0.8875 

25 

3.7 

0.8861 

28 

4.35 

.  .  . 

30 

4.601 

.  . 

33 

5.0 

.  . 

35 

5.17 

.  .  . 

40 

5.75 

45 

6.105 

50 

6.8 

55 

7.315 

.  .  . 

60 

7.9 

.  .  .  • 

65 

8.4 

.  . 

70 

8.898 

.  .  . 

75 

9.4 

81 

10.027 

(Christomanos.) 

716 


PHOSPHORUS 


Sol.  to  about  1%  in  acetic  acid.  (Vulpius, 
Arch.  Pharm.  1878,  213.  38.) 

100  g.  96%  acetic  acid  dissolve  0.105%  P. 
(Stich,  Pharm.  Ztg.  1903,  48.  343.) 

Sol.  in  0.05  pt.  CS2  (Bottger);  0.125  pt. 
(Trommsdorf.) 

Alcohol  ppts.  P  from  CS2  solution. 

1  pt.  CS2  dissolves  17-18  pts.  P.  (Vogel, 
J.  B.  1868.  149.) 

Solubility  in  CS2  at  t°, 
(g.  per  100  g.  of  solution.) 


t° 

G.P4 

t° 

G,P4 

-10 
-7.5 
-5 
-3.5 
-3.2 

31.40 
35.85 
41.95 
66,14 

71  .  72 

-2.5 
0.0 
+5.0 
+10.0 

75.00 

81.27 
86.30 
89.80 

(Cohen  and  Inouye,  Z.  phys.  Ch.  1910,  72. 

418.) 

Very  sol.  in  methylene  iodide.  (Retgers, 
Z.  anorg.  3.  343.) 

Strong    vinegar    dissolves    P.      (Beudet.) 

Sol.  in  considerable  amount  in  stearic  acid. 
(Vulpius,  Arch.  Pharm.  (3)  13.  38.) 

Sol.  in  ethyl  chloride,  benzoyl  chloride, 
stannic  chloride,  and  in  liquid  cyanogen. 

SI.  sol.  in  ethyl  nitrite,  and  wood-spirit. 

SI.  sol.  in  acetone,  with  gradual  decomposi- 
tion. 

Insol.  in  nicotine,  and  coniine. 

SI.  sol.  in  cold,  more  sol.  in  hot  benzene. 
(Mansfield.) 

Sol.  in  14  pts.  hot,  and  less  in  cold  petro- 
leum from  Amianp.  (Saussure.) 

SI.  sol.  in  "liquid  paraffine."  (Crismer,  B. 
17.  649.) 

SI.  sol.  in  warm  essential  oils,  as  oil  of  tur- 
pentine, and  in  the  fatty  oils. 

Sol.  in  hot  oil  of  copaiba,  separating  out  on 
cooling. 

Sol.  in  hot  oil  of  caraway,  and  mandarin 
oil.  (Luca.) 

SI.  sol.  in  cold,  more  sol.  in  hot  caoutchin, 
depositing  on  cooling. 

Readily  sol.  in  warm,  less  in  cold  styrene. 

Sol.  in  aniline,  and  quinoline.    (Hofmann.) 

SI.  sol.  in  cold  creosote. 

Somewhat  sol.  in  fusel  oil. 

Easily  sol.  in  valerianic  acid,  and  amyl 
valerate. 

Sol.  in  hexyl  alcohol,  ethylene  chloride, 
allyl  sulphocyanide,  mercury  methyl,  chloro- 
form, bromoform,  warm  chloral,  acetic  ether, 
aldehyde,  hot  cacodyl  sulphide,  and  in  cacodyl 
oxide. 

100  g.  oil  of  almonds  sat.  with  P  contain 
1.25  g.  (Stich,  C.  C.  1903,  I.  1291.) 

100  g.  oleic  acid  sat.  with  P  contain  1.06  g. 
(Stich.) 

100  g.  paraffine  sat.  with  P  contain  1.  g. 
(Stich.) 


(b)  Amorphous  phosphorus.    Insol.  in  H2O. 

Insol.  in  NH4OH+Aq.     (Fliickiger.) 

Sol.  in  boiling  KOH+Aq. 

The  statement  of  Burgess  and  Chapman, 
(Chem.  Soc.  79.  1235)  that  red  P  is  sol.  in 
aqueous  alcoholic  alkali  is  incorrect.  Both 
ordinary  crystalline  and  amorphous  red  P  are 
insol.  in  aqueous  alcoholic  alkali.  (Michaelis, 
A.  1902,  325.  367.) 

Insol.  in  liquid  NH3.  (Hugot,  A.  ch.  1900 
(7)  21,  31);  (Franklin,  Am.  Ch.  J.  1898,  20. 
828.) 

Bright  red  variety  is  sol.  in  liquid  NH3  at 
ord.  temp,  leaving  a  black  residue.  (Stoch, 
Bottcher  and  Lenger,  B.  1909,  42.  2854.) 

Red.    Amorphous. 

Sol.  in  S2C12  with  foaming.  (Nicolardot, 
C.  R.  1908,  147.  1304.) 

Solubility  of  amorphous  bright  red  P4 
in  PBr3  is  diminished  by  long  heating  as 
follows: 

172°  185° 

Initial  concentration  0 . 555         0 . 476 

Final  concentration  0 . 374         0 . 397 

Length  of  expt.  in  hours  34  24 

198°  218° 

0.592  0.476 

0.416  0.592 

18  17 

{Buck,  Dissert.  1904.) 

Ordinary  amorphous  P4  is  sol.  in  PBr3. 
A  sample  prepared  by  heating  bright  red 
amorphous  P    with  94.2%  P  dissolved  by 
heating  in  PBr3  as  follows: 

%P          0.106        0.121         0.178 
hours  10  20  42 

A  finely  pulverized  commercial  product 
containing  98.0%  P: 

%P  0.92  0.116 

hours  10  20 

An  ordinary  commercial  product  with 
98%  P: 

%P  0.056  0.108 

hours  10  42 

(Buck.) 

100  g.  PBr3  dissolve  0.2601  g.  bright  red 
phosphorus  at  172°;  0.3634  g.  at  184°. 
(Schenk,  B.  1902,  35.  353.) 

Insol.  in  KOH+Aq. 

Cone.  H2SO4  does  not  act  upon  it  in  the 
cold,  but  dissolves  easily  when  hot. 

Insol.  in  dil.,  easily  sol.  in  cone.  HNO3  + 
Aq  with  decomposition. 

Much  more  sol.  in  HNO3+Aq  than  ordi- 
nary P.  (Personne,  C.  R.  45.  115.) 

Insol.  in  methylene  iodide.     (Retgers.) 

Appreciably  sol.  in  isobutyl  alcohol. 
(Svedberg.) 

Insol.  in  CS2,  alcohol,  ether,  naphtha, 
ligroine,  PCls,  etc. 

SI.   sol.   in  boiling  oil   of  turpentine  and 


PHOSPHORUS  PLATINIC  CHLORIDE 


717 


other  high-boiling  liquids,  with  conversion 
into  ordinary  phosphorus. 

Insol.  in  oil  of  turpentine  even  at  270°. 
(Colson,  A.  ch.  1908,  (8)  14.  554.) 

(c)  Crystalline.  Insol.  in,  and  not  attacked 
by  dil.  HNO3+Aq. 

Sol.  in  CS2. 

Phosphorus  ^n'bromide,  PBr3. 

Decomposed  by  H2O,  slowly  at  8°,  but  very 
rapidly  at  25°.  (Lowig,  Pogg.  14.  485.) 

Sol.  in  liquid  H2S.  (Antony  and  Magri, 
Gazz.  ch.  it.  1905,  35.  (1)  206.) 

Sol.  in  AlBr3.  (Isbekow,  Z.  anorg.  1913, 
84.  27.) 

Sol.  in  ether,  acetone,  CHC13,  C6H6  and 
CS2.  (Christomanos,  Z.  anorg.  1904,  41.  287.) 

Phosphorus  pentabromide,  PBr6. 

Fumes  on  air,  and  is  violently  decomp.  by 
H20. 

Phosphorus  ^nbromide  ruthenium  bromide, 
Ru2P5Bri9. 

Decomp.  by  boiling  H2O. 

Slowly  sol.  in  hot  alcohol  with  decomp. 

Insol.  in  benzene,  CC14,  ligroin  and  cold 
alcohol.  (Strecker,  B.  1909,  42.  1775.) 

Phosphorus  thiophosphoryl  bromide,   PBr3, 

PSBr3. 
Decomp.  by  H2O  into  PSBr3.    (Michaelis.) 

Phosphorus    ^nbromide    ammonia,     3PBr3, 

5NH3. 

Slowly  but  completely  sol.  with  decomp.  in 
H2O.  (Storer's  Diet.) 

Phosphorus   pentabromide    ammonia.   PBr5, 

9NH3. 
(Besson,  C.  R.  111.  972.) 

Phosphorus  wonobromo^rachloride,  PBrCl4. 
Decomp.  by  H2O.     (Prinvault,  C.  R.  74. 
868.) 

Phosphorus  e&bromo/nchloride,  PCl3Br2. 
Very  unstable.    (Michaelis,  B.  5.  9.) 

Phosphorus  ^rabromo^nchloride,  PCl3Br4. 
Decomp.  with  H2O.    (Geuther.) 

Phosphorus    heptdbromodichlonde,  PCl2Br7. 
Very  unstable.    (Prinvault,  C.  R.  74.  868.) 

Phosphorus  octobromo^nchloride,  PCl3Br8. 
Very  easily  decomp.    (Michaelis,  B.  6.  9.) 

Phosphorus  bromofluoride,  PF3Br2. 

Decomp.  violently  with  H2O.  (Moissan, 
Bull.  Soc.  (2)  43.  2.) 


Phosphorus  bromonitride. 
See  Nitrogen  bromophosphide. 

Phosphorus  bichloride,  P2Cl4. 

Decomp.  by  H2O.  (Besson,  C.  R.  1910. 
150.  103.) 

Phosphorus  trichloride,  PC13 

Gradually  decomp.  by  H2O. 

0.11  g.  is  sol.  in  100  ccm.  liquid  H2S.  (An- 
tony, Gazz.  ch.  it.  1905,  35  .(1)  206.) 

Acted  upon  by  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  828.) 

Miscible  with  CS2,  C6H6,  CHC13,  and 
ether. 

Decomp.  with  alcohol. 

Phosphorus  pentochloride,  PC15. 

Very  deliquescent,  and  sol.  in  H2O  with 
violent  decomp.  and  evolution  of  heat.  Sol. 
in  liquid  HC1.  Acted  upon  by  liquid  NH3. 
Somewhat  sol.  without  decomp.  in  CS2. 
(Schiff,  A.  102.  118.  (Franklin,  Am.  Ch.  J. 
1898,  20.  828.) 

Sol.  without  decomp.  in  benzoyl  chloride. 
(Gerhardt.) 

Sol.  in  oil  of  turpentine  with  evolution  of 
heat. 

Monophosphorus    platinous    chloride,    PC13. 

PtCl2. 

Deliquescent.  Sol.  in  H2O  with  formation 
of  chloroplatinophosphoric  acid.  Similarly 
decomp.  by  alcohol.  Abundantly  sol.  in  hot 
benzene,  toluene,  chloroform,  or  carbon  tetra- 
chloride,  and  crystallizes  on  cooling.  (Schtit- 
zenberger,  Bull.  Soc.  (2)  17.  482.) 

Diphosphorus  platinous  chloride,  2PC13, 
PtCl2. 

Decomp.  by  H2O  with  formation  of  chloro- 
platinodiphosphoric  acid.  Similarly  decomp. 
by  alcohol.  Sol.  without  decomp.  in  PC13, 
CC14,  CHC13,  C6H6,  orC7H8.  (Schiitzen- 
berger.) 

Sol.  in  propyl  alcohol  with  formation  of 
the  propyl  ether  of  platinochlorophosphor- 
ous  acid  and  HC1.  (Pomey,  C.  R.  104.  364.) 

Phosphorus  diplatinous  chloride,  PC13, 

2PtCl2. 

Sol.  in  alcohol,  with  formation  of  ether 
(PtCl2)2P(OC2H5)3.  (Cochin,  C.  R,  86. 
1402.) 


Phosphorus  platinic  chloride,  PC13, 

(Schiitzenberger.) 


Phosphorus  pentachloride  platinic    chloride, 

PC16,  PtCl4,  or  (PCl4)2PtCl6. 
Decomp.  at  once  by  H2O.     (Baudrimont, 
A.  ch.  (4)  2.  47.) 


718 


PHOSPHORUS  SELENIUM  CHLORIDE 


Phosphorus     pentacbloride     selenium    tetra- 

chloride,  2PC15,  SeCl4. 
Sol.  in  H2O  with  decomp.     (Baudrimont, 

A.  ch.  (4)  2.  5.) 

Phosphorus  ^nchloride   ruthenium  chloride, 

Ru2P5Cl19. 

Slowly  decomp.  by  boiling  H2O. 
Sol.  in  benzene  and  CHC13. 
SI.  sol.  in  CC14.    Insol.  in  ligroin.    (Strecker, 

B.  1909,  42.  1774.) 

Phosphorus    tellurium    chloride,    PC15, 
2TeCl4. 

Very  deliquescent. 

Sol.  in  H2O.  (Metzner,  A.  ch.  1898,  (7) 
15.  203.) 

Phosphorus  pentochloride    stannic  chloride, 

PC15,  SnCl4. 

Very  deliquescent.  Sol.  in  much  H2O  with 
evolution. of  heat,  forming  SnCl4,  HC1,  and 
H3PO4,  and  soon  separates  out  stannic  phos- 
phate. (Casselmann,  A.  83.  257.) 

Phosphorus    ^nchloride    titanium    chloride, 

PC13,  Ti£l4. 
(Bertrand,  Bull.  Soc.  (2)  33.  565.) 

Phosphorus  pentachloride  titanium  chloride, 
PC16,  TiCl4. 

Deliquescent.  Decomp.  by  H2O  and  alco- 
hol. Sol.  in  ether.  SI.  sol.  in  PC13.  (Tiitts- 
chew,  A.  141.  111.) 

Completely  sol.  in  dil.  acids.    (Weber.) 

Phosphorus    uranium    perctachloride,    PC15, 

UC15. 
Decomp.  with  H2O. 

Phosphorus  pentacbloride  zirconium  chloride, 

PC15,  ZrCl4. 

Decomp.  by  H2O  with  pptn.  of  Zr  phos- 
phate. (Paykull.) 

Phosphorus    trichloride    ammonia,    PC13, 

5NH3. 

Insol.  as  such  in  H20,  but  slowly  decomp. 
by  boiling  H2O.  More  easily  sol.  with  de- 
comp. in  acids.  Sol.  with  decomp.  by  boiling 
with  KOH  or  NaOH  + Aq.  (Berzelius.) 

Phosphorus    pentacbloride    ammonia,    PC15. 

5NH3. 

Properties  as  PC13,  5NH3.     (Berzelius.) 
PC1B,  8NH3.    SI.  decomp.  on  air.    (Besson, 

C.  R.  111.  972.) 

Phosphorus  pentachLoride  tungsten  ^n'oxide, 

2PC15,  W03(?). 
(Persoz  and  Bloch,  C.  R.  28.  389.) 

Phosphorus   chlorobromide. 
See  Phosphorus  bromochloride. 


Phosphorus  chlorofluoride,  PC12F3. 

Absorbed  by  H2O  with  decomp.  Absorbed 
by  alcohol  or  ether.  (Poulenc,  A.  ch.  (6)  24. 

555.) 

Phosphorus  chloroiodide,  PC13I2. 

Decomp.  by  moist  air  or  H2O.  Sol.  in  CS2. 
(Most,  B.  13.  2029.) 

Phosphorus  chloronitride. 

See  Nitrogen  chlorophosphide. 

Phosphorus  ^fluoride,  PF3. 

Decomp.  slowly  by  H2O.  (Moissan,  Bull. 
Soc.  (2)  43.  2.) 

Rapidly  absorbed  by  KOH  or  NaOH+Aq, 
slowly  by  BaO2H2,  and  K2CO3+Aq.  Ab- 
sorbed by  absolute  alcohol  with  decomp. 
(Moissan,  C.  R.  99.  655.) 

Phosphorus  pentofluoride,  PF5. 

Fumes  on  air.    (Thorpe,  A.  182.  20.) 

Phosphorus    pentofluoride   ammonia,   2PF5, 

5NH3. 
(Moissan,  C.  R.  101.  1490.) 

Phosphorus  pentofluoride  nitrogen  peroxide. 
Decomp.  by  H2O.    (Tassel,  C.  R.  110. 1264. 

Phosphorus  fluobromide. 
See  Phosphorus  bromofluoride. 

Phosphorus  fluochloride. 
See  Phosphorus  chlorofluoride. 

Phosphorus  sw&iodide,  P4I. 

Sol.  in  dil.  HNO3  and  in  alkalies +Aq. 
(Boulouch,  C.  R.  1905,  141.  257.) 

Phosphorus  cftiodide,  P2I4. 

Decomp.  by  H2O.  Sol.  in  CS2.  (Coren- 
winder,  A.  ch.  (3)  30.  242.) 

0.09  g.  is  sol.  in  100  ccm.  liquid  H2S.  (An- 
tony, C.  C.  1906,  I.  1692.) 

Phosphorus  ^niodide,  PI3. 

Very  deliquescent.  Decomp.  in  moist  air 
and  by  H2O.  (Corenwinder,  A.  ch.  (3)  30. 

242.) 

Very  sol.  in  CS2. 

Phosphorus  pentaiodide,  PI5  (?). 
(Hampton,  C.  N.  42.  180.) 

Phosphorus  iodosulphide. 
See  Phosphorus  sulphoiodide. 

Phosphorus  nitride,  P3N5. 

Very  slightly  decomp.  by  long  boiling 
with  H2O. 

Completely  insol.  in  any  solvent.  (Stock, 
B.  1903,  36.  317.) 


PHOSPHORUS  SULPHIDE 


719 


Phosphorus  sw&oxide,  P4O. 

Unchanged  in  dry,  gradually  oxidized  in 
moist  air.  Insol.  in  H2O,  alcohol,  ether,  and 
oils;  not  acted  on  by  HCl+Aq;  oxidized  by 
HNO3  or  H2SO4.  (Marchand,  J.  pr.  13.  442.) 

SI.  sol.  in  H2O.    (le  Verrier,  A.  27.  167.) 

Forms  hydrate  P4O,  2H2O,  which  gives  up 
its  H2O  when  dried. 

Two  modifications:  (a)  decomp.  slowly  by 
H2O  or  alkalies,  (6)  not  decomp.  by  H2O  or 
alkalies.  (Reinitzer  and  Goldschmidt,  B.  13. 
847.) 

Is  oxyphosphuretted  hydrogen  (?), 
P4H(OH).  (Franke,  J.  pr.  (2)  35.  341.) 

H3P50. 

Insol.  in  all  solvents.  Decomp.  by  H2O. 
Not  attacked  by  non-oxidizing  acids.  De- 
comp. by  dil.  alkalies.  (Gautier,  C.  R.  76. 
173.) 

P4HO. 

Insol.  in  nearly  all  substances.  Not  at- 
tacked by  dilute  acids;  oxidized  by  ordinary 
HNO3,  and  cone.  H2SO4  at  200°.  Attacked 
by  very  dil.  alkaline  solutions.  Perhaps 
identical  with  phosphorus  suhoxide  P4O. 
(Gautier,  C.  R.  76.  49.) 

Phosphorus  oxide,  P2O. 

Decomp.  by  heating  with  H2O  at  100°. 
(Besson,  C.  R.  1897,  124.  764.) 

Phosphorus   dioxide,    P4O6(formerly   P2O3), 
Deliquescent,  but  very  slowly  dissolved  by 

cold  H2O  to  form  H3P03.    Violently  decomp. 

by  hot  H2O  or  alcohol. 

Sol.  without  decomp.  in  ether,  carbon  disul- 

phide,  benzene,  or  chloroform.    (Thorpe  and 

Tutton,  Chem.  Soc.  57.  545.) 

Phosphorus  teZroxide,  P2O4. 

Very  deliquescent.  Sol.  with  evolution  of 
heat  in  H2O.  (Thorpe  and  Fulton,  Chem. 
Soc.  49.  833.) 

Phosphorus  pentoxide,  P2Os. 

Very  deliquescent.  Sol.  in  H2O  with  great 
evolution  of  heat,  forming  H3PO4. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
Q.  1014);  (Naumann,  B.  1904,  37.  4329.) 

Phosphorus    sulphur    oxide,    P2O5,    3SO3  = 

(PO)2(SO4)3(phosphoryl  sulphate)  (?). 
Decomp.  by  H2O.    Sol.  in  cold,  more  sol.  in 
warm  SO3.    (Weber,  B.  20.  86.) 

Phosphorus  oxy-compounds. 

See  under  Phosphoryl  compounds. 


Phosphorus  oxy sulphide. 
See  Phosphorus  sulphoxide. 

Phosphorus  semiselenide,  P4Se. 

Decomp.  with  H2O.  Insol.  in  cold,  de- 
comp. by  boiling  KOH+Aq.  Insol.  in,  but 
apparently  decomp.  by  alcohol  and  ether. 
Easily  sol.  in  CS2.  (Harm,  J.  pr.  93.  430.) 

Phosphorus  monoselenide,  P2Se. 

Stable  in  dry,  decomp.  in  moist  air  and  by 
H2O.  Insol.  in  alcohol  and  ether.  Decomp. 
by  boiling  KOH+Aq.  CS2  dissolves  out  P. 
(Hahn,  J.  pr.  93.  430.) 

SI.  sol.  in  CS2.  (Gore,  Phil.  Mag.  (4)  30. 
414.) 

Phosphorous  sesgmselenide,  P4Se3. 

Sol.  in  CCli;  si.  sol.  in  CS2.  (Meyer,  7. 
anorg.  1902,  30.  258.) 

Phosphorus  ^nselenide,  P2Se3. 

Decomp.  by  boiling  H2O  and  slowly  in 
moist  air.  Easily  sol.  in  cold  KOH+Aq, 
less  easily  in  M2CO3+Aq.  Insol.  in  alcohol, 
ether,  and  CS2.  (Hahn,  J.  pr.  93.  430.) 

Phosphorus  pentoselenide,  P2Se5. 

Slowly  decomp.  in  moist  air  or  by  H2O, 
easily  by  KOH+Aq  or  alcohol.  Insol.  in 
CS2.  Sol.  in  CC14.  (Hahn,  J.  pr.  93.  430.) 

Phosphorus  selenides  with  M2Se. 
See  M  phosphoselenide,  under  M. 

Phosphorus  semisulphide,  P4S(?). 

1.  Liquid.    Not  decomp.  by,  and  insol.  in 
boiled  H2O.    Insol.  in  alcohol  and  ether.    SI. 
sol.   in  fats  and  volatile  oils;  decomp.   by 
alkalies.      Dissolves    P    on    warming,    with 
separation  on  cooling.    Sol.  in  CS2. 

2.  Red    modification.     Not     attacked    at 
first  by  HNO3+Aq  (sp.  gr.  1.22),  but  after 
a  time  is  attacked  with  the  greatest  violence. 
Weak  acids  attack  only  when  hot.     (Berze- 
lius,  A.  46. 129.) 

Existence  is  doubtful.  (Schulze,  B.  13. 
1862;  Isambert,  C.  R.  96.  1628.) 

Phosphorus  monosulphide,  P2S(?). 

1.  Ordinary.      Same   properties    as   phos- 
phorus semsulphide,  1. 

2.  Red  modification.      Unchanged  by  air, 
H2O,  or  alcohol.    Decomp.  by  cone.  KOH  + 
Aq,  not  by  dilute.     SI.  sol.  in  NH4OH+Aq. 
(Berzelius,  A.  46.  129.) 

Existence  is  doubtful.  (Schulze;  Isam- 
bert.) 

Does  not  exist.  (Helff,  Z.  phys.  Ch.  12. 
206.) 

Phosphorus  sesgwisulphide,  P4S3. 

Not  attacked  by  cold,  slowly  by  hot  H2O. 
Cold  KOH+Aq  dissolves  with  decomp. 


720 


PHOSPHORUS  SULPHIDE 


Oxidized  by  HNO3  and  aqua  regia.  Sol.  in 
alcohol  and  ether  with  decomp.  Sol.  in  CS2 
(100  pts.  CS2  dissolve  60  pts.  P4S3),  PC13,  and 
PSC13.  and  in  K2S  or  Na2S+Aq.  (Lemoine, 
Bull.  Soc.  (2)  1.  407.) 

Very  sol.  in  CS2.    (Rebs,  A.  246.  367.) 
Decomp.    by   dil.    and    cone.    KOH+Aq. 
1  pt.  P4S3  is  sol.  in  9  pts.  CS2  at-20°;  in 
3.7  pts.  CS2  at  0°;  in  1  pt.  CS2  at  17°;  in  40 
pts.  benzene  at  17°;  in  9  pts.  benzene  at  80°; 
in  32  pts.  toluene  at  17°;  in  6.5  pts.  toluene  at 
111°.    (Stock,  B.  1910,  43.  156.) 

Phosphorus  Zn'sulphide,  P2S3. 

Decomp.  by  water.    (Kekule*,  A.  90.  310.) 
Sol.  in  M2CO3+Aq  with  separation  of  S. 

Easily  sol.  in  KOH,  NaOH,  NH4OH+Aq. 

(Berzelius,  A.  46.  129.) 
Sol.  in  alcohol  and  ether.     (Lemoine.) 
Correct  formula  is  P4S6.    (Isambert,  C.  R. 

102.  1386.) 

Extremely  si.  sol.  in  CS2.     (Rebs,  A.  246. 

368.) 

Existence  doubtful.     (Helff,  Z.  phys.  Ch. 

12.  210.) 

Phosphorus  sulphide,  P4S7. 

SI.  sol.  in  CS2.    (Mai,  A.  265.  192.) 

Slowly  decomp.  by  cold,  rapidly  by  hot 
H2O. 

Sol.  in  cold  alkalies. 

1  pt.  is  sol.  in  3500  pts.  CS2  at  17°;  in  20,000 
pts.  at  0°.  (Stock,  B.  1910,  43.  416.) 

Phosphorus  bisulphide,  P3S6  (formerly  P2S4). 
Almost  insol.  in  CS2.     (Helff.) 

Phosphorus  pentasulphide,  P2S5. 

Very  deliquescent.  Decomp.  by  H2O. 
Very  sol.  in  KOH,  NaOH,  NH4OH+Aq. 
Sol.  in  M2CO3+Aq  with  separation  of  S  at 
low  temp.  Decomposes  alcohol,  acetic  acid, 
etc.  (Kekul<§,  A.  106.  331.) 

Sol.  in  CS2.    (Isambert,  C.  R.  102.  1386.) 

Not  very  sol.  in  CS2.    (Rebs,  A.  246.  367.) 

Mpt.,  290°;  bpt.,  513-515°  at  760  mm. 

Decomp.  by  H2O. 

Easily  sol.  in  warm  NaOH+Aq. 

1  pt.  is  sol.  in  450  pts.  CS2  at  room  temp.; 
in  550  pts.  at  0° ;  in  1200  pts.  at — 20°.  (Stock, 
B.  1910,  43.  1225.) 

Ordinary  form. 

Sol.  in  195  pts.  boiling  CS2. 

New  form. 

Sol.  in  32  pts.  CS2.  (Stock,  B.  1905,  38. 
2722.) 

Phosphorus  persulphide,  P2Si2  (?). 

Decomp.  by  H2O,  alkalies,  etc.  Consist's 
of  S,  and  mechanically  united  P.  (Ramme, 
B.  12.  941.) 

Phosphorus  sulphides  with  M2S. 
See  M  Phosphosulphide,  under  M. 


Phosphorus  zinc  sulphide,  ZnP3S2. 

Sol.  in  HCl+Aq  with  separation  of  P3S  (?). 
(Berzelius,  A.  46.  150.) 

Phosphorus  ^'sulphide  ammonia,  P2S3,  2NH8. 
Decomp.  by  H2O.    (Bineau.) 

Phosphorus   pentosulphide   ammonia, 

P2S5,  6NH3. 

Sol.  in  liquid  NH3.  (Stock,  B.  1903,  36. 
314.) 

P2S5,  7NH3.    (Stock.) 

Phosphorus   sulphobromide. 
See  Thiophosphoryl  bromide. 

Phosphorus  sulphochloride. 
See  Thiophosphoryl  chloride. 

Phosphorus  sulphoiodide,  P2S3I. 

SI.  attacked  by  cold,  rapidly  by  hot  H2O; 
violently  decomp.  by  fuming  HNO3.  Easily 
sol.  in  CS2.  SI.  sol.  in  C6H6  or  CHC13,  and 
still  less  in  ether  or  absolute  alcohol.  (Ouv- 
rard,  C.  R.  115.  1301.) 

P2S2I2.  Easily  sol.  in  CS2.  More  easily 
than  P4S3I2  and  less  than  PI3.  (Ouvrard,  A. 
ch.  1894,  (7)  2.  224.) 

P2SI4.    Easily  decomp.    (Ouvrard.) 

P4S3I2.  Insol.  in  H2O;  sol.  in  warm  ether. 
SI.  sol.  in  benzene,  CHCls  and  glacial  acetic 
acid;  sol.  in  toluene  and  xylene.  (Wolter,  Ch. 
Ztg.  1907,  31.  640.) 

Easily  sol.  in  CS2.  SI.  sol.  in  benzene,  ether, 
absolute  alcohol  and  CHC13.  (Ouvrard,  C.  R. 
1892,  115.  1301.) 

Phosphorus  sulphoxide,  P4O6S4. 

Deliquescent.  Easily  sol.  in  H2O  with  de- 
comp. Sol.  in  2  pts.  CS2  without  decomp. 
Sol.  in  benzene  with  decomp.  (Thorpe  and 
Tutton,  Chem.  Soc.  59.  1019.) 

P202S3.  Slowly  decomp.  by  H2O.  Vio- 
lently attacked  by  fuming  HN03.  (Besson, 
C.  R.  1897,  124.  152.) 

P4S3O4.  Deliquescent;  sol.  in  H20  with 
decomp.;  insol.  in  most  solvents.  (Stock,  B. 
1913,  46.  1382.) 

Phosphoryl  Jn'amide,  PO(NH2)3. 

Insol.  in  boiling  H2O,  KOH+Aq,  or  diL 
acids.  Decomp.  by  long  boiling  with  HC1  or 
HNO3-|-Aq.  More  easily  decomp.  with 
aqua  regia.  Easily  sol.  in  warm  H2SO4  or 
nitrosulphuric  acid.  (Schiff,  A.  101.  300.) 

Does  not  exist.  (Gladstone;  Mente,  A. 
248.  238.) 

Phosphoryl  bromide,  POBr3. 

Not  miscible  with  H2O,  but  gradually  de- 
comp. in  contact  with  it.  Sol.  in  H2SO4, 
ether,  oil  of  turpentine  (Gladstone,  Phil. 
Mag.  (3)  35.  345);  in  CHC13,  CS2  (Baudri- 
mont,  Bull.  Soc.  1861.  118). 


PHOSPHOTELLURATE,  AMMONIUM 


721 


Easily  sol.  in  AsBr 
1902,  29.  374.) 


(Walden,  Z.  anorg. 


Sol.  in  CC14,  and  in  C6H6.  (Oddo,  Chem. 
Soc.  1900,  78.  (2)  75.) 

Phosphoryl  bromide  sulphide. 
See  Thiophosphoryl  bromide. 

Phosphoryl  bromochloride,  POCl2Br. 

Decomp.  by  H2O.  (Menschutkin,  A.  139. 
343.) 

Phosphoryl   cfaibromochloride,   POClBr2. 

Decomp.  by  H2O.  (Geuther,  Jena  Zeit. 
10.  130.) 

Phosphoryl  chloride,  POC1. 

Very  hygroscopic.  Sol.  in  H2O  with  de- 
comp.  Insol.  in  most  solvents.  Sol.  in  PC13. 
(Besson,  C.  R.  1897,  125.  772.) 

POC13.  Decomp.  by  H2O.  Not  acted  on 
by  liquid  CO2,  P,  PH3,  CS2,  I,  Br,  Cl,  etc. 
Sol.  in  CC14,  C6H6,  CS2,  CHC13  and  ether. 
(Oddo,  Gazz.  ch.  it.  1899,  29.  (2)  318;  Chem. 
Soc.  1900,  78  (2)  74.) 

Phosphoryl  boron  chloride,  POC13,  BC13. 
See  Boron  phosphoryl  chloride. 

Phosphoryl  stannous  chloride,  POC13,  SnCl2. 
Deliquescent.    Decomp.  by  H2O     (Cassel- 
mann,  A.  91.  242.) 

Phosphoryl  stannic  chloride,  POC13>  SnCl4. 

Deliquescent.  Decomp.  by  H2O.  (Cassel- 
mann.) 

Phosphoryl  titanium  chloride,  POC13,  TiCl4. 

Deliquescent,  and  decomp.  by  H2O. 
(Weber,  Pogg.  132.  453.) 

Pyrophosphoryl  chloride,  P2O3C14. 

Decomp.  violently  with  H2O.  (Geuther 
and  Michaelis,  B.  4.  766.) 

Very  sol.  in  H2O  with  decomp.;  very  un- 
stable. (Besson,  C.  R.  1897,  124.  1100.) 

Metophosphoryl  chloride,  PO2C1. 
Decomp.  by  H20.    (Gustavson.) 
Does  not  exist.    (Michaelis.) 

Phosphoryl  fluoride,  POF3. 

Absorbed  and  decomp.  at  once  by  H2O  or 
alcohol.  (Moissan,  C.  R.  102.  1245.) 

Phosphoryl  imidoamide,  PN2H3O  = 

PO(NH)NH2. 

Insol.  in  H2O;  gradually  decomp.  by  boiling 
with  H2O,  more  rapidly  in  presence  of  KOH. 
Insol.  in  boiling  cone.  HCl+Aq.  Insol.  in 
cold,  decomp.  by  hot  H2SO4.  Moderately 
dil.  H2SO4+Aq  dissolves  without  evolution 


of  gas.     Insol.  in  boiling  nitric  or  nitrosul- 
phuric  acid.    (Gerhardt,  A.  ch.  (3)  20.  255.) 
Insol.  in  alcohol,  oil  of  turpentine,  etc. 

Phosphoryl  iodide,  P3I6O8  (?). 

Sol.  in  H2O,  alcohol,  and  ether.     (Burton, 
Am.  Ch.  J.  3.  280.) 

PO2I2.    (Burton.) 

Phosphoryl  nitride,  PON. 

Insol.  in  H2O,  acids,  or  alkalies.     (Glad- 
stone, Chem.  Soc.  2.  121.) 

Phosphoryl  chlorosulphide,  P2O2SC14. 

Slowly    decomp.    in    contact    with    H2O. 
(Besson,  C.  R.  1897,  124.  153.) 

Phosphoryl  thio-campounds. 
See  Thiophosphoryl  compounds. 

Phosphoselenic  acid. 

See  Selenophosphoric  acid. 

Phosphoselenide,  M. 
See  under  M. 

Phosphosilicic  acid. 
See  Silicophosphoric  acid. 

Phosphosilicosovanadicotungstic  acid. 

Ammonium    phosphosilicosovanadicotung- 

state. 

Exact  formula  not  known.     (E.  F.  Smith, 
J.  Am.  Chem.  Soc.  1903,  26.  1225.) 

Phosphosilicovanadic  acid,  3SiO2,  2V2O6, 

2P2O6+6H2O. 
Sol.  in  H2O.    (Berzelius.) 

Phosphostannosovanadicotungstic  acid. 

Ammonium     phosphostannosovanadicotung- 
state. 

Exact  formula  not  known.     (E.  F.  Smith, 
J.  Am.  Chem.  Soc.  1903,  26.  1226.) 

Phosphosulphide,  M. 

See  under  M. 

Phosphosulphuric  anhydride,  P2O6,  3SO8. 

Very  easily  decomp.    (Weber,  B.  19.  3190.) 

Phosphotelluric  acid. 

Ammonium  phosphotellurate,  2(NH4)2O, 
P2O5,  TeO3+4H2O. 

Easily  sol.  in  H2O.     (Weinland,  Z.  anorg. 
1901,  28.  61.) 

4(NH4)2O,  3P2O5,  2TeO3  +  llH2O.    Sol.  in 
H2O  without  decomp.    (Weinland.) 


722 


PHOSPHOTELLURATE,  POTASSIUM 


Potassium  phosphotellurate,   1.5K2O,   P2O6, 
TeO3. 
+17.5  H2O.    Very  sol.  in  H2O. 
+4.5  H2O.    Ppt.    (Weinland.) 

Rubidium  phosphotellurate,  1.5Rb2O,  P2O5, 
TeO3+4.5H2O. 
Ppt.    (Weinland.) 

Sodium  phosphotellurate,  2Na2O,  P2O5, 
2TeO3+9H2O. 
Difficultly  sol.  in  cold  H2O.    (Weinland.) 

Phosphothorosovanadicotunstic  acid. 

Ammonium  phosphothorosovanadicotung- 
state. 

Exact  formula  not  known.     (E.  F.  Smith, 
J.  Am.  Chem.  Soc.  1903,  25.  1226.) 

Solubility  in  H2O  at  t°. 

t° 

100  ccm.  H2O  dis- 
solve g.  of  the 
cryst.  acid 

Sp.  gr.  of  the 
solution 

0 
22 
43 
92 

16.206 
49.718 
53.64 

86.75 

1.1890 
1.6913 
1.8264 
2.5813 

(Soboleff,  Z.  anorg.  1896,  12.  31.) 
Solubility  in  ether  at  t°. 

t° 

100  ccm.  ether  dissolves  g.  of 
the  cryst.  acid. 

0 

7. 
18. 
24. 

8 
2 
2 

81.196 
85.327 
96.017 
101  .  348 

Phosphotitanosovanadicotunstic  acid. 

Ammonium  phosphotitanosovanadicotung- 

state. 

Formula  not  known.  (E.  F.  Smith,  J.  Am. 
Chem.  Soc.  1903,  25.  1226.) 

Phosphotungstic  acid,  P2O5,  12WO3+ 
42H2O. 

Not  efflorescent.  Sol.  in  H2O,  alcohol,  and 
ether.  (PSchartf,  C.  R.  110.  754.) 

P2O5,  16WO3+69H2O.  Very  efflorescent. 
Sol.  in  H2O,  alcohol,  and  ether.  (Pe*chard, 
C.  R.  109.  301.) 

+zH2O  =  HsPWgO;*  +zH2O  (o-phospholu- 
teotungstic  acid).  Known  only  in  aqueous 
solution.  (Kehrmann,  B.  20.  1808.) 

+48H2O  =H3PW8O28  +  16H2O  (a-anhydro- 
phospholuteotungstic  acid) .  Sol.  in  its  crystal 
H2O  by  warmth  of  the  hand;  sol.  in  less  than 
Vs  pt.  H2O.  (Kehrmann.) 

Correct  composition  is  represented  by 
H3PW9O31+9H2O.  (Kehrmann,  Z.  anorg.  1. 
422.) 

P2O5,  20WO3+8H2O.  Very  efflorescent. 
(Gibbs,  B.  10.  1386.) 

+19H2O  =  HnPW10O38+8H2O.  Sol.  in 
H2O.  (Scheibler,  B.  5.  801.) 

+50,  and  62H2O.  Very  efflorescent. 
(P6chard,  C.  R.  109.  301.) 

3H2O,  P2O5,  21WO3+30H2O.  Efflores- 
cent. Sol.  in  H2O  in  nearly  every  proportion. 

P2O5,    22WO3+28H2O=HBPW1iO43  + 
18H2O.    Efflorescent.    (Scheibler,  B.  5.  801.) 

Composition  is  6H2O,  22WO3,  P2O5+ 
45H2O.  (Gibbs.) 

H3PO4, 12WO3  +  18H2O,  or  P2O5,  24WO3  + 
39H2O.  Sol.  in  H2O,  alcohol  and  ether. 
(Soboleff,  Z.  anorg.  1896,  12.  18.) 

P2O5,    24WO3+40H2O  =  6H2O,    P2O5, 
24WO3+34H2O.     Very  efflorescent.     Sol.  in 
H2O.    (Gibbs.) 

+45H2O. 


(Soboleff.) 

+53H2O=6H2O,  P2O5,  24WO3+47H2O. 
Sol.  inH2O.  (Gibbs.) 

Sol.  in  ether.  If  an  equal  vol.  of  ether  is 
placed  above  a  layer  of  cone,  aqueous  solution 
of  acid,  oily  drops  form  between  the  two 
layers,  which  sink  to  bottom,  forming  a  third 
layer.  The  sp.  gr.  of  the  latter  is  1.525.  The 
crystallized  acid  dissolved  in  smallest  amt. 
ether  forms  an  oil  of  sp.  gr.  =2.083.  Ethereal 
solution  is  miscible  with  alcohol,  and  also 
with  a  large  quantity  of  H2O.  (Drechsel,  B. 
20.  1452.) 

+61H2O.  Sol.  in  H2O.  (Gibbs,  Proc. 
Am.  Acad.  16.  116.) 

Aluminum  ammonium  phosphotungstate. 

See  Aluminicophosphotungstate,  ammo- 
nium. 

Ammonium  phosphotungstate,  3(NH4)2O, 

P205,  7W03+Aq. 

SI.  sol.  in  cold  H2O  without  decomp.  De- 
comp.  by  hot  H2O.  (Kehrmann,  Z.  anorg. 

1892,  1.  438.) 

2(NH4)2O,  P2O6,  12WO3+5H2O.  Insol.  in 
cold  H20.  (Pochard,  C.  R.  110.  754.) 

6(NH4)2O,  P2O6,  16WO3+10H2O.  Easily 
sol.  in  hot  H2O.  (Pe'chard.) 

5(NH4)2O,  P2O5,  16WO3+zH2O  = 
(NH4)5PW8O29+zH2O.    (Ammonium  a-phos- 
pholuteotungstate).    SI.  sol.  in  H2O.    (Kehr- 
mann.) 

3(NH4)2O,  P2O5,  16WO3  +  16H2O  = 
(NH4)3PW8O28+8H2O.      (Ammonium   a-an- 
hydrophospholuteotungstate) .      Efflorescent. 
Easily  sol.  in  H2O.    (Kehrmann.) 

5(NH4)2O,  P2O5,  17WO3  +  16H2O.  Very 
si.  sol.  in  cold  H2O.  (Kehrmann,  Z.  anorg. 
1894,  6.  387.) 

3(NH4)20,  P206,  18W03+14H20.  (Phos- 
pholutestungstate.)  (Kehrmann,  Z.  anorg. 

1893,  4.  140.) 


PHOSPHOTUNGSTATE,  POTASSIUM 


723 


3(NH4)2O,  P2Os,  2lWO3+zH2O.  Rather 
si.  sol.  in  cold,  easily  in  hot  H2O  and  alcohol 
Insol.  in  sat.  NH4Cl+Aq.  (Kehrmann  and 
.Freinkel,  B.  25.  1972.) 

3(NH4)2O,  3H2O,  P2O5,  22WO3  +  18H2O. 
SI.  sol.  in  cold  H2O.  (Gibbs.) 

3(NH4)2O,  3H2O,  P2O5,  24WOs+26H2O. 
Very  si.  sol.  even  in  hot  H2O.  (Gibbs,  Proc. 
Am.  Acad.  16.  122.) 


Ammonium    barium    a-anhydrophospholuteo- 
tungstater  NH4BaPW8O2*+zH2O  = 
(NH4)2O,  2BaO,  P2O5,  16WO3+zH2O. 
Sol.  in  H2O.    (Kehrmann.) 

Barium  phosphotungstate,  2BaO,  P2O5, 
12WO3  +  15H2O. 

Very  efflorescent.  Sol.  in  H2O;  insol.  in 
alcohol.  (Pechard,  C.  R.  110.  754.) 

3BaO,  P2O5,  16WO3+zH2O  =  Ba3(PW8O2S) 
4-#H2O.  (Barium  a-anhydrophospholuteo- 
tungstate).  Not  efflorescent.  Quite  diffi- 
cultly sol.  in  H2O.  (Kehrmann.) 

2BaO,P2O5,  16WO3  +  10H2O.  Efflorescent. 
(Pochard,  A.  ch.  (6)  22.  240.) 

2BaO,  6H2O,  P2O5,  20WO3+24H2O.  Sol. 
in  H2O.  (GiBbs,  B.  10.  1386.) 

6BaO,  2H2O,  P2O5,  20WO3+46H2O.  Sol. 
in  H2O.  (Gibbs,  Proc.  Am.  Acad.  16.  126.) 

7BaO,  P2O5,  22WO3+59H2O.  Sol.  in  H20, 
(Sprerger,  J.  pr.  (2)  22.  418.) 

+53H2O.    (Kehrmann,  B.  24.  2335.) 

4BaO,  2H2O,  P2O5,  22WO3+39H2O.  Sol. 
m  H2O  without  decomp.  (Gibbs.) 

BaO,  P2O5,  24WO3+59H2O.  Sol.  in  H2O. 
(Sprenger.) 

2BaO,  P2O5,  24WO3+59H2O.  Sol.  in  H20. 
(Sprenger.) 

3BaO,  P205,  24WO3+46H2O  =3BaO,  3H2O, 
P2O5,  24WO3+43H2O.  Easily  sol.  in  hot  H2O. 
(Gibbs.) 

3BaO,  P2O5,  24WO3+48H2O.  Sol.  in  H2O. 
(Soboleff,  Z.  anorg.  1896,  12.  18.) 

+58H2O.    Sol.  in  H2O.    (Sprenger.) 

Efflorescent.  SI.  sol.  in  dil.  BaCl2+Aq. 
(Kehrmann,  Z.  anorg.  1.  423.) 

Barium  potassium  phosphotungstate.  5BaO. 

2K2O,  P2O5,  22WO3+48H2O. 
Sol.  in  H2O.     (Kehrmann  and  Freinkel,  B. 
25.  1968.) 

Barium   silver   phosphotungstate,   4BaO 

3  Ag2O,  P2O6,  22WO3+34H2O. 
Very   si.    sol.    in   H2O.      (Kehrmann   and 
Freinkel,  B.  25.  1966.) 

Barium    sodium    phosphotungstate,    2BaO, 

Na2O,  P2O5,  24WO3+46H2O. 
Sol.  in  H2O,  forming  cloudy  liquid,  which 
clears  up.     Solution  in  HC1  is  not  cloudy. 
(Brandhorst  and  Kraut,  A.  249.  380.) 


Calcium  phosphotungstate,  CaO,  5H2O, 
16WO3,  P2O5+3H2O. 

Readily  sol.  in  H2O.  (Gibbs,  Proc.  Am. 
Acad.  16.  130.) 

2CaO,  P2O6,  12WO3+19H2O.  Efflores- 
cent. Insol.  in  alcohol.  (Pochard,  C.  R.  110. 
754.) 

2CaO,  P2O,  20WO3+22H2O.  Efflores- 
cent. (Pochard,  A.  ch.  (6)  22.  233.) 

Cadmium    phosphotungstate,    2CdO,    P2O5, 

12WO3  +  13H2O. 

SI.  efflorescent.  Very  sol.  in  H2O.  (P6- 
chard,  C.  R.  110.  754.) 

Cupric     phosphotungstate,  3CuO,     24WO3, 

P2O5+58H2O. 

Sol.  in  H2O.    (Sprenger,  J.  pr.  (2)  22.  418.) 
2CuO,  P2O5,  12WO3  +  11H2O.  Very  efflores- 
cent.   (Pochard,  C.  R.  110.  754.) 

2CuO,  P2O5,  20WO3  +  13H2O.  Efflores- 
cent. (Pe*chard,  A.  ch.  (6)  22.  235.) 

Lead  phosphotungstate,  2PbO,  P2O5,  12WO3 
+6H20. 

Insol.  in  cold,  sol.  in  boiling  H2O.  (Pe*- 
chard,  C.  R.  110.  754.) 

2PbO,  P2O5, 20WO3+6H2O.  Sol.  in  boiling 
H2O.  (Pochard,  A.  ch.  (6)  22.  236.) 

Lithium  phosphotungstate,   Li2O,   P2O5, 

12W03+21H20. 
Sol.  in  H2O.    (Pochard,  C.  R.  110.  754.) 

Magnesium  phosphotungstate,  2MgO,  P2O6/ 

12WO3. 

SI.  efflorescent.    (P4chard,  C.  R.  110.  754.) 
2MgO,  P2O5,  20WO3  +  19H2O.    SI.  efflores- 
cent.   (Pochard,  A.  ch.  (6)  22.  234.) 

Mercurous  phosphotungstate. 

Insol.  in  dil.  HNO3+Aq.  (Pochard,  C.  R. 
110.  754.) 

Potassium  phosphotungstate,  K2O,  P2O5, 
12WO3+9H2O. 

Insol.  in  cold,  si.  sol.  in  hot  H2O.  (Pochard, 
C.  R.  110.  754.) 

5K2O,  P2O5,  16WO3+zH2O  =  K5PW8O29-f- 
zH2O.  (Potassium  a-phospholuteotungstate) . 
Very  si.  sol.  in  cold,  more  easily  in  hot  H2O. 
Sol.  in  cold  dil.  HN03+Aq.  (Kehrmann.) 

3K2O,  P2O5,  16WO3  +  16H2O=K3PW8O29 
+8H2O.  (Potassium  a-anhydrophospho- 
luteotungstate) .  Efflorescent.  Easily  sol. 
in  H2O.  (Kehrmann.) 

5K2O,  P2O5,  17WO3+21  or  22H2O.  SI. 
sol.  in  cold  H2O.  (Kehrmann,  Z.  anorg. 
1894,  6.  387.) 

3K2O,  P2O5,  18WO3+28H2O.  (Duparc 
and  Pearce,  Bull.  Soc.  Min.  1895,  18.  42.) 

K2O,  5H2O,  P2O6,  18WO3  +  14H2O,  Very 
si.  sol.  in  H2O.  (Gibbs.) 

6K2O,  P2O5,  18WO3+30H2O,  and  23H20. 


724 


PHOSPHOTUNGSTATE,  POTASSIUM  LEAD 


The  23H2O  salt  is  more  sol.  in  H2O  than  the 
30H2Osalt.  (Gibbs.) 

7K2O,  H2O,  P2O6,  20WO3+27H2O.  Sol.  in 
H2O.  (Gibbs,  B.  10.  1386.) 

K2O,  P2O5,  20WO3+5H2O.  Nearly  insol. 
in  H2O.  (Pochard,  A.  ch.  (6)  22.  231.) 

8K2O,  P2O5,  20WO3  +  18H2O.  SI.  sol.  in 
H2O.  (Gibbs.) 

3K2O,  P2O5,  21WO3+31H2O.  Easily  sol. 
in  cold  H2O  or  alcohol.  Much  less  sol.  in  very 
dil.  HC1  + Aq  or  KC1  +Aq.  Decomp.  by  boil- 
ing H2O.  (Kehrmann  and  Freinkel,  B.  25. 
1971.) 

2K2O,  4H2O,  P2O5,  22WO3+2H2O.  Very 
si.  sol.  in  H2O.  (Gibbs.) 

7K2O,  P2O5,  22WO3+31H2O.  Easily  sol. 
in  cold  or  hot  H2O.  Insol.  in  alcohol.  (Kehr- 
mann, B.  25.  1966.) 

3K2O,  3H2O,  P2O6,  24WO3+8,  and  14H2O. 
Sol.  in  a  large  amount  of  H2O  with  partial  de- 
comp.  (Gibbs;  Proc.  Am.  Acad.  16.  120.) 

Practically  insol.  in  H2O.  Easily  sol.  in 
NH4OH,  alkalies,  or  alkali  carbonates +Aq. 
(Kehrmann,  B.  24.  2329.) 

6K2O,  P2O6,  24WO3  +  18H2O.  Sol.  in  H2O. 
(Gibbs,  Proc.  Am.  Acad.  15.  1.) 

Potassium  lead  a-phosphoZwteotungstate. 
SI.  sol.  in  H2O.    (Kehrmann.) 

Silver  phosphotungstate,  Ag2O,  P2OS,  12WO3 
+8H2O. 

Ppt.  Insol.  in  H2O.  (Pochard,  C.  R.  110. 
754.) 

5Ag2O,  P2O5,  16WO3+zH2O=Ag5PW8O29 
•+zH2O  (Silver  a-phospholuteotungstate) . 
Ppt.  (Kehrmann.) 

3Ag2O,  P2O6,  16WO3+16H2O=Ag3PW8O28 
+8H2O.  (Silver  a-anhydrophospholuteo- 
tungstate).  Easily  sol.  in  H2O.  (Kehrmann.) 

Ag2O,  24WO3,  P2O5+60H2O.  Insol.  in 
H2O. 

3Ag2O.  24WO3,  P2O6+58H2O.  Insol.  in 
H2O.  (Sprenger,  J.  pr.  (2)  22.  418.) 

Sodium  phosphotungstate,  3Na2O,  P2O5, 
7WO3+Aq. 

Sol'in  H2O.    (Kehrmann,  Z.  anorg.  1. 437.) 

5Na2O,  11H2O,  2P2O5,  12WO3+26H2O  = 
Na5HnP2W6O31-|-13H2O  (?).  (Scheibler,  B. 
5.  801.) 

2Na2O,  P205,  12WO3  +  18H2O.  Sol.  in 
H2O.  Insol.  in  alcohol.  (Pochard,  C.  R.  110. 
754.) 

5Na2O,  14WO3,  2P2O5+42H2O.  Easily 
sol.  in  H2O.  (Gibbs.) 

Na2O,P2O5,20WO3,2H2O+19H20.  Sol.  in 
H2O.  (Gibbs,  Am.  Ch.  J.  1895,  17.  183.) 

Na2O,  P2O5, 20WO3+23H2O  =  Na2O, 7H2O, 
P2O5.  20WO3  +  16H2O.  Easily  sol.  in  H2O. 
(Gibbs.) 

+25H2O.  SI.  efflorescent;  very  sol.  in 
H2O;  insol.  in  alcohol.  (Pochard,  A.  ch.  (6) 
22.  227.) 

2Na2O,  P2O5, 20WO3  +  10H2O.  Sol.  in  H20; 
insol.  in  alcohol.  (Pe*chard.) 


+30H2O.    (P.) 

3Na2O,  P2O6,  20WO3+32H2O.    As  above. 

(P.) 

2Na2O,  P2O5,  22WO3+9H2O.  Very  si.  sol. 
in  H2O.  (Gibbs.) 

3Na2O,  P2O5,  24WO3+22H2O.  Sol.  in  H2O. 
(Brandhorst  and  Kraut,  A.  249.  379.) 

+30H2O.  Sol.  in  H2O.  (Soboleff,  Z. 
anorg.  1896,  12.  18.) 

+42H2O. 

Solubility  in  H2O  at  t°. 


t° 

100  ccm.  H2O  dissolve  g. 
of  the  cryst.  salt 

0 
22 
93 

22.04 
59.65 

98.184 

(Soboleff,  Z.  anorg.  1896,  12.  31.) 

2Na2O,  4H2O,  24WO3,  P2O5+23H2O. 
Readily  sol.  in  H2O.  (Gibbs,  Proc.  Am.  Acad. 
16.  118.) 

Sp.  gr.  at  20°  of  solutions  of  2Na2O,  4H2O, 
P2O6,  24WO3+23H2O  containing: 

10.22  20.94  31.13%  salt, 

1.085  1.190  1.3^6 

42.61  52.92  64.11%  salt. 

1.496             1.702  2.001 
or,  by  calculation,  a  =  sp.  gr.  if  %  is  crystal- 
lized salt,  b  =  sp.  gr.  if  %  is  anhydrous  salt: 

5  10  15          20          25%  salt, 

a    1.040     1.084      1.131  1.181      1.237 

b  1.044     1.092      1.143  1.199      1.262 

30          35          40          45          50%  salt, 
a    1.299      1.370      1.449      1.538      1.640 
b   1.333      1.414      1.507      1.613      1.734 

55          60         64%  salt, 
a    1.754     1.884     1.998 
b   1.872      ... 
(Brandhorst  and  Kraut,  A.  249.  377.) 

Strontium    phosphotungstate,    2SrO,    P2O5, 

12WO3  +  17H2O. 

Sol.  in  H2O.  Insol.  in  alcohol.  (Pochard, 
C.  R.  110.  754.) 

Thallium     phosphotungstate,     T12O,     P2O6, 

12WO3+4H2O. 
Ppt.    (Pochard,  C.  R.  110.  754.) 

Zinc  phosphotungstate,  2ZnO,  P2O5,  12WO3 

7H2O. 
Efflorescent.    (Pochard,  C.  R.  110.  754.) 

Monometaphosphotungstic  acid. 

Ammonium  wonowetaphosphotungstate, 

(NH4)2O,  2NH4PO3,  18WO3  +  11H2O. 
SI.  sol.  in  cold  H2O. 


PHOSPHOVANADICOZIRCONOSOTUNGSTATE,  AMMONIUM 


725 


Potassium  monowetaphosphotungstate, 

3K2O,  2KPO3,  24WO3+20H2O. 
Very  si.  sol.  in  H2O.    (Gibbs,  Am.  Ch.  J.  7. 
319.) 

Orthometaphosphotungstic  acid. 

Potassium     sodium     orthometaphosphotung- 
state,  2K2O,  4Na2O,  6NaPO3,  6K3PO4, 
22WO3+42H2O. 
SI.  sol.  in  H2O.    (Gibbs,  Am.  Ch.  J.  7.  319.) 

Ps/rophosphotungstic  acid. 

Ammonium   manganous    sodium    pyrophos- 
photungstate,  5(NH4)2O,  6MnO,  2Na2O, 
2P2O5,  28WO3+48H2O. 
Very  sol.  in  cold  and  in  hot  H2O.    (Gibbs, 

Am.  Ch.  J.  1895,  17.  90.) 

Ammonium    sodium     pi/rophosphotungstate, 
6(NH4)4P2O7,      3Na4P2O7,      2(NH4)2O, 
22WO3+31H2O. 
Nearly  insol.  in  cold  H2O  or  NH4OH+Aq. 

Sol.  in  a  large  amount  of  hot  H2O. 

Manganous    sodium    pyrophosphotungstate, 

6Na2O,  3MnO,  P2O5,  14WO3+36H2O. 
Efflorescent  in  dry  air.     Sol.  in  H2O  and 
can  be  recryst.  therefrom.    (Gibbs.) 

Potassium  ps/rophosphotungstate,  9K4P2O7, 
22WO3+49H2O. 

Very  si.  sol.  in  cold  H2O. 

6K4P2O7,  3H4P2O7,  22WO3,  K2O,  H2O  + 
42H2O.  SI.  sol.  in  cold.  Sol.  in  much  boiling 
H2O.  (Gibbs,  Am.  Ch.  J.  7.  392.) 

Phosphovanadic  acid,  P2O5,V2O5, 2H2O+ 
9H20. 

Sol.  in  H2O. 

Composition  is  vanadium  phosphate 
(VO2)H2PO4+4^H2O.  (Friedheim,  B.  23. 
1531.) 

This  is  the  only  "acid"  which  exists.    (F.) 

P2O5,  V2O5+14H2O.  Sol.  in  H2O;  can  be 
recryst.  from  dil.  H3PO4+Aq.  (Ditte,  C.  R. 
102.  757.) 

3P2O5,2V2O6+9H2O.  Sol,inH2O.  (Ditte.) 

P2O5,  3V2O5.    (Berzelius.) 

3H2O,  7P2O5,  6V2O5+34H2O.  Sol.  in  H2O. 
Decomp.  by  much  H2O  into — 

6H2O,  P2O6,  20V2O6+53H2O.  Sol.  in  H2O. 
(Gibbs,  Am.  Ch.  J.  7.  209.) 

Ammonium  phosphovanadate,  (NH4)2O, 
P205,  V205+H20. 

SI.  sol.  in  cold  H20.  (Gibbs,  Am.  Ch.  J. 
7.  209.) 

+3H2O.  Composition  is  (VO2)(NH4)HPO4 
+H2O.  (Friedheim.) 

(NH4)2O,  P2O5,  2V2O5+7H2O.  Easily  sol. 
in  H2O.  (Gibbs.)  SI.  sol.  in  H2O.  (Fried- 


heim.) Composition  is  (NH4)2O,  V2O5, 
+2(VO2)H2PO4+5H2O.  (Friedheim.) 

5(NH4)2O,  2P2O5,  3V2O5+24H2O.  Easily 
sol.  in  H2O.  (Ditte,  C.  R.  102.  1019.)  Could 
not  be  obtained.  (Friedheim.) 

5(NH4)2O,  4P2O5,  2V2O5+24H2O.  As 
above.  (Ditte.)  Could  not  be  obtained. 
(Friedheim.) 

7(NH4)2O,  P2O5,  12V2O5+26H2O.  Easily 
sol.  in  H2O.  Composition  is  2(NH4)2HPO4  + 
5(NH4)2O,  12V2O6+25H2O.  (Friedheim.) 

Potassium    phosphovanadate,     K2O.     P2O5, 

2V2O5+7H2O. 

SI.  sol.  in  H2O;  decomp.  thereby  to  7K2O, 
12V2O5,  P2O5+26H2O. 

Composition  is  K2O,  V2O8+2(VO2)H2PO4 
+5H2O.  (Friedheim.) 

3K2O,  4P2O5,  6V2O6+21H2O.  SI.  sol.  in 
H2O.  (Gibbs.) 

7K2O,  P2O6,  12V2O5+26H2O.     Easily  sol. 
in  H2O.     Composition  is  2K2HPO4+5K2O, 
12V2O5+25H2O.    (Friedheim.) 
2K2O,  P2O5,  V2O5. 
3K2O,  2P2O5,  2V2O5+5H2O. 
13K2O,  2P2O5,  22V2O5+58H2O. 
15K2O,  2P2O5,  25V2O5+76H2O. 
(Friedheim,  Z.  anorg.  1894,  5.  446.) 
16K2O,  2P206,  27V2O5+57H2O. 
6K2O,  P2O5,  11V2O5+33H2O. 
7K2O,  P2O6,  13V2O6+38H2O. 
4K2O,  P2O5,  3V2O5+3H2O. 
(Friedheim,  Z.  anorg.  1894,  6.  459-465.) 

Silver  phosphovanadate,  2Ag2O,  P2O5,  V2O5  + 

5H2O. 
SI.  sol.  in  cold  or  hot  H2O.    (Gibbs.) 

Phosphovanadicotungstic  acid. 

Ammonium  phosphovanadicotungstate, 
(NH4)2O,  P2O5,  V2O3,  WO3+zH2O. 

Ppt.  (Smith,  J.  Am.  Chem.  Soc.  1902,  24. 
577.) 

15(NH4)20,  2P205,  6V203,  44WO3  + 
106H2O.  Sol.  in  H2O.  Insol.  in  alcohol, 
ether  or  benzene.  (Rogers,  J.  Am.  Chem. 
Soc.  1903,  25.  303.) 

Phosphovanadicovanadiotungsticacid. 

Ammonium  phosphovanadicovanadiotung- 
state,  14(NH4)2O,  2P2O5,  3V2O3,  7V2O5, 
27WO3+66H2O. 
Sparingly  sol.  in  cold  H2O.    Sol.  in  hot  H2O. 

(Rogers,  J.  Am.  Chem.  Soc.  1903,  26.  309.) 

Phosphovanadicozirconosotungstic  acid. 

Ammonium    phosphovanadicozirconosotung- 
state. 

Exact  formula  not  known.  (E,.  F.  Smith 
J.  Am.  Chem.  Soc.  1903,  25.  1226!) 


726 


PHOSPHOVANADICOVANADIC  ACID 


Phosphovanadicovanadic  acid. 

Ammonium  phosphovanadicovanadate, 

7(NH4)2O,  2P2O6,  VO2,  18V2O5+50H2O. 
Sol.  in  H2O.    (Gibbs,  Am.  Ch.  J.  7.  209.) 
7(NH4)2O,  14P2O5,  16VO2,  6V2O5-f-65H2O. 

Decomp.  by  boiling  with  H2O  into — 

5(NH4)2O,  10P2O5,  11VO2,  V2O6+41H2O. 

Sol.  inH2O.    (Gibbs.) 

Potassium ,  5K2O,  12P2O6,  12VO2,  6V2O6 

+40H20. 

Decomp.  by  hot  H2O  into — 

7K2O,  12P2O5,  14VO2,  6V2O5+52H2O. 
Sol.  inH2O.  (Gibbs.) 

Sodium  ,  4Na2O,  5P2O6,  VO2,  4V2O6  + 

37H2O. 
Insol.  in  H2O.    (Gibbs.) 

Phosphovanadiomolybdic  acid. 

Ammonium  phosphovanadiomolybdate, 
7(NH4)2O,   2P2O5,  V2O5,  48MoO3  + 
30H2O. 

SI.  sol.  in  cold,  somewhat  more  in  hot  H2O 
with  partial  decomp.  (Gibbs,  Am.  Ch.  J.  6. 
391.) 

8(NH4)2O,  P2O6,  8V2O5,  14MoO3+50H2O. 
Easily  sol.  in  hot  H2O  without  decomp. 
(Gibbs.) 

5(NH4)2O,  P2O6,  2^V2O6,  2l^MoO3  + 
50H2O. 

8(NH4)2O,  P2O5,  5V2O5,  18MoO3+45H2O. 

7(NH4)2O,  P2O5,  5y2VzO5,  16^Mo03  + 
50H2O. 

8(NH4)2O,  P2O5,  7V2O5,  15MoO3+50H2O. 

All  above  compounds  are  sol.  ih  H2O. 
(Blum,  J.  Am.  Chem.  Soc.  1908,  30.  1859.) 

6(NH4)2O,  P2O6,  7V2O5,  9MoO3+28H2O, 
+33H2O,  and  +37H2O. 

Can  be  recryst.  from  H2O.  (Hinsen,  Dis- 
sert. 1904.) 

4(NH4)2O,  P2O5,  4V2O5,  HMoO3+37H2O. 
(Jacoby,  Dissert.  1900.) 

6(NH4)2O,  P2O5,  7V2O6,  HMoO3+34H2O 
and+43H2O.  (Hinsen,  Dissert.  1904.) 

8(NH4)2O,  P2O6,  7V2O5,  HMoO3+30H2O. 
(Hinsen.) 

5(NH4)2O,  P2O5,  4V2O6,  12MoO3+39H2O. 
1  cc.  of  solution  in  H2O  contains  0.2624  g. 
of  hydrous  salt.  Sp.  gr.  of  solution  at  18°  = 
1.0932.  (Lahrmann,  Dissfert.  1904.) 

6(NH4)2O,  P2O5,  4V2O5,  12MoO3+24H2O. 
Nearly  insol.  in  cold  H2O.  (Lahrmann.) 

7(NH4)2O,  P2O5,  6V2O5,  12MoO3+33H2O. 
(Stamm,  Dissert.  1906.) 

6(NH4)2O,  P2O5,  4V2O6,  13MoO3+37H2O. 
1  cc.  of  solution  sat.  at  18°  contains  0.1543  g. 
hydrous  salt  and  has  sp.  gr.  =  1.0900.  (Tog- 
genburg,  Dissert.  1902.) 

6(NH4)2O,  P2O5,  5V2O5,  13MoO3+29H20. 
1  cc.  solution  sat.  at  18°  contains  0.2533  g. 
hydrous  salt.  Sp.  gr.  =  1.0797.  (Stamm, 
Dissert.  1906.) 


+32H2O.     (Stamm.) 

+34H2O.      Stamm.) 

6(NH4)2O,  P2O5,  4V2O5,  14MoO3+28H2O. 
Easily  sol.  in  H2O  with  decomp.  (Toggen- 
burg,  Dissert.  1902.) 

8(NH4)2O,  P2OS,  4V2O5,  14MoO3+24H2O. 
Decomp.  by  cold  H20.  (Lahrmann,  Dissert. 
1904.) 

5(NH4)2O,  P2O5,  3V2O5,  5MoO3+39H2O. 
1  cc.  of  solution  sat.  at  18°  contains  0.2445 
g.  hydrous  salt  and  has  sp.  gr.  =  1.144.  (Ja- 
coby, Dissert.  1900.) 

6(NH4)2O,  P2O6,  3V205,  15  MoO3+41H2O. 
Extraordinarily  easily  sol.  in  H20.  (Ja- 
coby.) 

7(.NH4)2O,  P2O6,  3  2O5,  18MoO3+31H2O. 
(Schulz  Dissert.  1905.) 

6(NH4)2O,  P2O5,  3V2O5,  18MoO3+40H2O. 
(Schulz.) 

8(NH4)2O,  P2O5,  5V2O  ,  73MoO3+26H2O. 
+33H2O.  (Stamm,  Dissert  1905.) 

Ammonium    barium    ,  0.5(NH4)2O, 

5.5BaO,   P2O5,   6V2O5,   8MoO3+38H2O. 
(Hinsen,  Dissert.  1904.) 

2(NH4)*O,  4BaO,  P2O5,  7V2O5,  10  MoO3  + 
43H2O.  SI.  sol.  in  H2O.  Decomp.  on  heating. 
(Toggenburg,  Dissert.  1902.) 

(NH4)2O,  5BaO,  P2O5,  6V2O5,  12MoO3  + 
49  H20.  Less  sol.  in  H2O  than  NH4  comp. 
(Jacoby,  Di^sert.  1900.) 

2(NH4)20,  4BaO,  P2O5,  4V2O5,  13MoO3  + 
37  H2O.  Sol.  in  much  hot  H20  with  decomp. 
(Toggenburg,  Dissert.  1902.) 

2(NH4)2O,  4BaO,  P2O5,  5V2O5,  13MoO3+ 
46H2O.  (Stamm,  Dissert.  1905.) 

3  NH4)2O,  4BaO,  P2O5,  5V2O5,  13MoO3  + 
40H2O.  (Stamm.) 

3(NH4)2O,  3BaO,  P2O5,  4V2O5,  14MoO3  + 
39H2O.  (Stamm.) 

2(NH4)2O,  4BaO,  P2O5,  3V  O5,  17MoO3  + 
46H2O.  (Schulz,  Dissert.  1906.) 

Ammonium  potassium ,  (NH4)2O,  6K2O, 

P206,  6V2O6,  10  MoO3+38H2O. 

(Jacoby,  Dissert.  1900.) 

(NH4)2O,  6K2O,  P2O5,  7V2O6,  HMoO3  + 
25H2O.  (Jacoby,  Dissert.  190\) 

(NH4)2O,  5K2O,  P2O5,  6V2O5,  12MoO3  + 
46H2O.  (Jacoby.) 

(NH4)26,  5K2O,  P2O5.  5V2O5,  13MoO3  + 

+25H2O;+29H2O;  +30H2O.  SI.  sol.  in 
cold,  more  easily  in  hot  H2O.  (Stamm, 
Dissert.  1905.) 

5K2O,  (NH4)2O,  P2O5,  4V2O5,  14Mo03  + 
31  2O.  (Stamm.) 

(NH4)2O,  4K2O,  P2O5,  3V2O5,  15MoO3  + 
36H2O.  (Jacoby,  Dissert.  1900.) 

(NH4)2O,  6K2O,  P2O5,  3V2O5,  18MoO3  + 
43H2O.  (Schulz.  Dissert.  1906.) 

5(NH.-)oO,  K2O,  P2O5,  2V2O5,  20MoO3  + 
52H2O.  (Schulz.) 

Barium  potassium ,  2BaO,  2K20,  P2O5, 

2V206,  18  MoOs+47H2O. 
(Schulz,  Dissert.   1905.) 


PLATINATE,  BARIUM,  BASIC 


727 


Potassium  phosphovanadiomolybdate,  7K2O 
P2O5,  7V2O5,  9MoO3+25H2O. 

(Hinsen,  Dissert.  1904.) 

5K2O,  P2O5,  2V2O5,  20MoO3+53H2O 
(Schulz,  Dissert.  1905.) 

Phosphovanadiotungstic  acid. 

Ammonium    phosphovanadiotungstate, 
10(NH4)2O,    3P2O5,    V2O5,    60WO3 
60H2O. 

Nearly  insol  in  cold,  si.  sol.  in  hot  H2O 
Sol.  in  (NH4)2HPO4+Aq,  and  in  NH4OH  + 
Aq. 

5(NH4)2O,  P2O5,  3V2O5,  16WO3+37H2O 
Easily  sol.  in  H2O.  (Gibbs,  Am.  Ch.  J.  5 
391.) 

13(NH4)2O,  2P2O6,  8V2O5,  34WO3+86H2O 
Very  sol.  in  cold  and  hot  H2O. 

nsol.  in  alcohol,  ether,  CS2,  benzene  anc 
nitrobenzene.  (Rogers,  J.  Am.  Chem.  Soc 
1903,  25.  299.) 

Banum  ,  ISBaO,  3P2O6,  2V2O  ,  60WO 

+  144H2O. 

Easily  sol  in  hot  H2O  with  decomp 
(Gibbs,Am.Ch.J.6.391.) 

Potassium 3K2O,  P2O6,  V2O5,  7WO3  + 

11H2O. 

Sol.  in  H2O. 

8K2O,  3P2O6,  4V2O5,  18WO3+23H2O.  Sol 
in  hot  H/J  with  decomp.  into  preceding  salt 
(Gibbs,  Am.  Ch.  J.  5.  391.) 

SUver ,  13Ag20,  2P206,  8V20£,  33WO8+ 

41H2O. 

Somewhat  sol.  in  H2O. 

Completely  sol.  in  H2O  containing  a  few 
drops  HNO3.  (Rogers,  J.  Am.  Chem.  Soc. 
1903,  25.  302.) 

Phosphovanadiovanadicotungstic  acid. 

Barium    phosphovanadiovanadicotungstate, 
18BaO,    3P2O5,    VOS,    VO2,    60WO3  + 
150H2O. 
SI.   sol.   in  cold,   easily  sol.   in  hot  H2O. 

(Gibbs,  Am.  Ch.  J.  5.  391.) 

Phosphuretted  hydrogen. 

See  Hydrogen  phosphide. 

Platibromonitrous  acid. 

Potassium  platibromonitrite,  K2Pt(N02)4Br2. 

Rather  si.  sol.  in  H2O.  (Blomstrand,  J.  pr. 
(2)  3.  214.) 

Sol.  in  about  40  pts.  cold,  and  20  pts.  boil- 
ing H2O.  Insol.  in  alcohol.  SI.  sol.  in  KBr  or 
KNO2+Aq.  (Vezes,  A.  ch.  (6)  29.  198.) 

K2Pt(NO2)8Br3.  Sol.  in  about  5  pts.  warm 
H2O  with  decomp.  (Vezes.) 


K2Pt(NO2)2Br4.  Sol.  in  less  than  5  pts. 
H2O  with  decomp.  (Vezes.) 

Platichloronitrous  acid. 

Potassium  platichloronitrite,  K2Pt(NO2)4Cl2. 

Rather  si.  sol.  in  H2O.  (Blomstrand  J.  pr. 
(2)3.214.) 

Sol.  in  40  pts.  cold,  and  20  pts.  boiling  H2O. 
Insol.  in  alcohol  SI.  sol.  in  KC1  or  KNO2  + 
Aq.  (Vezes,  A.  ch.  (6)29.  183.) 

K2Pt(NO2)8Cl3.   Very  sol.  in  H2O.    (Vezes.) 

K2Pt(NO2)Cl*+H2O.  Sol.  in  H2O  with 
decomp.  (Vezes.) 

Platiiodonitrous  acid. 

Potassium  platiiodonitrite,   K2Pt(NO2)2I4. 

SI.  sol.  in  cold,  more  easily  in  hot  H2O;  de- 
comp. by  boiling.  (Veze  ,  A.  ch.  (6)  29. 

207.) 

K2Pt(NO2)I5.     As  above.     (Vezes.) 

Platin-. 

See  also  Pla  ino-,  plato-,  p'at-,  and  platos-. 

Platincfo'amine  compounds. 

See  Chloro-,  bromo-,  hydroxylo-,  iodo-,  ni- 
rato-,  nitrito-,  sulphate-,  etc.,  platincfa'amine 
compounds. 

Platin^namine  carbonate, 

Pt(NH3)6(C03)2. 

Ppt.  Sol.  in  NaOH+Aq.  (Geddes,  J.  pr. 
(2)  26.  257.) 

-chloride    Pt(NH3)6Cl4. 
Sol.  in  hot  H2O     (Gerdes.) 

chloroplatinate,  Pt(NH3)  C14,   PtCl4-{- 

2H2O. 
Very  si.  Bol.  in  H2O.     (Gerdes.) 

-  nitrate,  Pt(NH3)6(NO8)4. 

Easily  sol.  in  H2O;  si.  sol.  in  HNO3+Aq. 

(Gerdes.) 

-  sulphate,  Pt(NH3)6(S04)2+H20. 
Nearly  insol.  in  H2O.    (Gerdes.) 

Mraplatinamine  iodide,  Pt4(NH3)8I10. 
(Blomstrand,  B.  16.  1469.) 

Ocfoplatinamine  iodide,  Pt8(NH3)i6Ii8. 

(Blomstrand.) 

Platinic  acid. 

Barium  platinate,  basic  (?),  3BaO,  2Pt02. 

Insol.    in    HC2H3O2+Aq;     easily    sol.    in 
HCl+Aq.    (Rousseau.) 


728 


PLATINATE,  BARIUM 


Barium  platinate,  BaPtO3. 

(Rousseau,  C.  R.  109.  144.) 

+H2O.  Insol.  in  dil.  HNO3+Aq;  sol.  in 
warm  HCl+Aq.  (Topsoe,  B.  3.  464.) 

+4H2O.  Very  si.  sol.  in  H2O,  BaO2H2,  or 
NaOH-f  Aq.  Easily  sol.  in  dil.  acids,  except 
HC2H3O2,  in  which  it  is  insol.  in  the  cold, 
but  decomp.  on  heating.  (Topsoe,  I.  c.) 

Composition  is  3BaPtO3,  BaCl2,  PtCl2O  + 
4H2O  (?).  (Johannsen,  A.  156.  204.) 

Calcium  platinate  chloride  (?),  2Ca2Pt2O5Cl2 
+7H20  (?). 

"Herschel's  precipitate." 

Easily  sol.  in  HCl+Aq,  and  in  HNO3+Aq, 
if  freshly  pptd.  (Herschel.  * 

Very  sol.  in  HNO3+Aq.  (Weiss  and 
Dobereiner,  A.  14.  252.) 

Composition  is  CaPtO3  PtCl2O,  CaO  + 
7H2O  (?).  (Johannsen,  A.  155.  204.) 


Potassium  platinate. 

Sol.  in  H2O.    (Berzelius.) 
K2O,   PtO2+3H2O.     V 


sol.   in   H20. 


.ry2w,     JTivy2-rojn.2v^.        very     t. 

(Blondel,  A.  ch.  1905,  (8)  6.  90.) 

K2Pt(OH)6.  Sol.  in  H2O;  insol.  in  alcohol. 
(Bellucci,  Z.  anorg.  1905,  44.  173.) 

Sodium  platinate,  Na2O,  3PtO2+6H2O. 

Dil.  acids  dissolve  out  Na2O  and  leave  PtO2. 
Sol.  in  HNO3+Aq.  (Dobereiner,  Pogg.  28. 
180.) 

Na20,  Pt02+3H20.  Sol.  in  H2O.  (Blon- 
del.) 

Afetoplatinic  acid,  5Pt02,  5H2O. 

Insol,  in  H20.  (Blondel,  A.  oh.  1905,  (8) 
6. 103.) 

Sodium  wetoplatinate,  Na2O,  5PtO2+9H2O. 
Insol.  in  H2O.     (Blondel.) 

Platinimolybdic  acid,  4H2O,  PtO2, 10MoO3, 
(Gibbs.) 

Ammonium  platinimolybdate, 

8Mo03,  2Pt02,  3(NH4)20  +  12H20. 

4MoO3,  2PtO2,2(NH4)20+19H2O. 

Sol.  in  hot  H2O.  (Gibbs,  Am.  Ch.  J.  1895, 
17.  80-82.) 

Potassium   platinimolybdate, 

60Mo03,  PtO2,  10K2O+40H2O. 
So  .  in  hot  H2O.     (Gibbs.) 

Silver  platinimolybdate. 

Sodium     platinimolybdate,     4Na2O,     PtO2 

10  MoO8-f29H20. 

Sol.  in  H2O.  (Gibbs,  Sill.  Am.  J.  (3)  14 
61.) 


Platinitungstic  acid. 

Ammonium  platinitungstate,  4(NH4)2O,  PtO2, 

10WO3+12H2O. 
Sol.  in  H2O.    (Gibbs,  B.  10.  1384.) 

Potassium    platinitungstate,    4K2O,  PtO2, 

10WO3+9H2O. 
Sol.  in  H2O.     (Gibbs.) 

Sodium  platinitungstate,  4Na2O,  PtO2, 
10WO8+25H2O. 

Sol.  in  H2O.    (Gibbs.) 

5Na2O,    7WO3,    2PtO2+35H2O.      Sol.    in 
H2O.     (Gibbs.) 

Is  double  salt  3Na2O,  7WO3+2Na2PtO3. 
Rosenheim,  B.  24.  2397.) 

10WO3,  PtO2,  4Na2O+23H2O. 

10WO3,  PtO2,  6Na2O+28H2O. 

20WO3,  PtO2,  9Na2O+58H2O. 

30WO3,  2PtO2, 15Na2O+89H2O. 

30WO3,  PtO2,  12Na2O+72H2O. 

All  are  sol.  in  boiling  H2O.  (Gibbs,  Am. 
Ch.  J.  1895,  17.  74-80.) 

Platino-. 

See  also  Plato — . 

Platinochlorophosphoric  acid. 

See  Chloroplatinophosphoric  acid. 

Platinocyanhydric  acid,  H2Pt(CN)4. 

Deliquescent.  Very  sol.  in  H2O,  alcohol, 
and  ether. 

Ammonium  platinocyanide,  (NH4)2Pt(CN)4 
+3H2O. 

Very  sol.  in  H2O. 

+2H2O.  Sol.  in  1  pt.  H2O,  and  still  more 
easily  in  alcohol. 

+H20. 

Ammonium  hydroxylamine  platinocyanide, 

NH4(NH4O)Pt(CN)4+3^H20. 
Sol.  in  H2O.    (Scholz,  M.  Ch.  1.  900.) 

Ammonium  magnesium  platinocyanide, 

(NH4)2Mg[Pt(CN)4]2+6H20. 

Barium  platinocyanide,  BaPt(CN)4+4H2O. 

Sol.  in  33  pts.  H2O  at  16°,  and  in  much  less 
at  100°.  Sol.  in  alcohol. 

Barium  potassium  platinocyanide, 

BaK2[Pt(CN)4]2. 
Sol.  in  H2O. 

Barium  rubidium  platinocyanide, 

BaRb2[Pt(CN)4]2. 
Sol.inH2O. 


PLATINOCYANIDE,  PRASEODYMIUM 


729 


Cadmium    platinocyanide,    CdPt(CN)4. 

Ppt.    Sol.  in  NH4OH+Aq.     (Martius,  A. 
117.  376.) 

CdPt(CN)4,  2NH3+H2O.     (M.) 

Calcium  platinocyanide,  CaPt(CN)4+5H2O. 
Very  sol.  in  H2O. 

Calcium  potassium  platinocyanide, 

CaK2[Pt(CN)4]2. 
Sol.  in  H2O. 

Cerium    platinocyanide,     Ce2[Pt(CN)4]3  + 

18H2O. 
Sol.  in  H2O. 

Cobaltous  platinocyanide  ammonia, 

CoPt(CN)4,  2NH3. 
Insol.  in  H2O,  but  sol.  in  hot  NH4OH+Aq. 

Cupric  platinocyanide,  CuPt(CN)4+sH2O. 
Ppt. 

Cupric  platinocyanide  ammonia,  CuPt(CN)4, 

2NH3+H2O. 

CuPt(CN)4,  4NH3.     Sol.  in  H2O,  alcohol, 
and  ether. 

Didymium    platinocyanide,    Di2[Pt(CN)4]3  + 

18H2O. 

Efflorescent    in    dry    air.      Sol.    in    H2O. 
(Cleve.) 

Dysprosium  platinocyanide,  Dy2[Pt(CN)4]3  + 

21H2O. 
Easily  sol.  in  H2O.    (Jantsch,  B.  1911,  44. 

1277.) 

Erbium    platinocyanide,    Er2[Pt(CN4)]3  + 

21H2O. 
Sol.  in  H2O.    (Cleve.) 

Gadolinium  platinocyanide, 

2Gd(CN),,  3Pt(CN)2+18H2O. 
Sol.  in  H2O;  decomp.  in  the  ah1.     (Bene- 
dicks, Z.  anorg.  1900,  22.  405.) 

Glucinum    platinocyanide,    GlPt(CN)4. 
(ToczynsU,  Dissert.  1871.) 

Hydroxylamine  platinocyanide, 

(NH4O)2Pt(CN)4+2H2O. 
Deliquescent.    Very  sol.  in  H2O.    (Scholz.) 

Hydroxylamine   lithium   platinocyanide, 

(NH4O)LiPt(CN)4+3H2O. 
Sol.  in  H2O. 

Indium  platinocyanide, 

In2[Pt(CN)4]3+2H2O. 
Hydroscopic;  sol.  in  H2O.    (Renz,  B.  1901, 
34.  2765.) 


Lanthanum     platinocyanide,     La2[Pt(CN)4]3 

+  18H20. 
Easily  sol.  in  H2O.    (Cleve.) 

Magnesium    platinocyanide,    MgPt(CN)4+ 

2H2O. 

Solubility  in  H2O. 

100  g.  of  the  sat.  solution  contain  at: 
96.4°  100° 

44 .33  43 . 96  g.  MgPt(CN)4 

(Buxhoevden,  Z.  anorg.  1897,  15.  325.) 

+4H20. 

Solubility  in  H2O. 

100  g.  of  the  sat.  solution  contain  at: 
42.2°    46.3°     48.7°       55° 
40.21    39.79    40.75    40.02  g.  MgPt(CN)4, 

58.1°       69°      77.8°     87.4° 

42.01  43.48  44.88  45.52  g.  MgPt(CN)4, 

93° 

45.04g.MgPt(CN)4. 
(Buxhoevden.) 


90° 
45.59 


+7H2O.  Sol.  in  3.4  pts.  H2O  at  16°. 
Easily  sol.  in  alcohol  and  ether. 

Solubility  in  H2O. 

100  g.  of  the  sat.  solution  contain  at: 
—4.12°  +0.5°  5.5°     18.0° 

24.9    26.33    28.07  31.23  g.  MgPt(CN)4, 

36.6°      45.0°      46.2° 
38 .36      41 . 32      41 . 96  g.  MgPt(CN)4. 
(Buxhoevden.) 

Magnesium  potassium  platinocyanide, 

MgK2[Pt(CN)4]2+7H2O. 
Sol.  in  H2O. 

Mercuric  platinocyanide,  HgPt(CN)4. 
Ppt. 

Mercuric  platinocyanide  nitrate,  5HgPt(CN)4 
Hg(NO3)2  +  10H2O. 

Ppt. 

Nickel  platinocyanide  ammonia,  NiPt(CN)4, 
2NH3+H20. 

Potassium  platinocyanide,  K2Pt(CN)4+ 
'3H2O. 

Extremely  efflorescent.  SI.  sol.  in  cold, 
easily  in  hot  H2O.  (Willm,  B.  19.  950.) 

Sol.  in  alcohol  and  ether. 

Potassium  sodium  platinocyanide,  K2Pt(CN)4, 

Na2Pt(CN)4+6H20. 
Sol.  in  H2O.    (Willm,  B.  19.  950.) 

Praseodymium  platinocyanide, 

2Pr(CN)3,  3Pt(CN)2. 

Sol.  in  H2O.  (Von  Scheele,  Z  anorg.  1898, 
18.  355.) 


730 


PLATINOCYANIDE,  SAMARIUM 


Samarium     platinocyanide,      Sm2[Pt(CN4)]3 

+  18H2O. 
Sol.inH2O.    (Cleve.) 

Scandivun  platinocyanide,  Sc2[Pt(CN)4]3 
+21H20. 

Sol.  in  H2O  and  insol.  in  alcohol;  when 
boiled  in  alcohol  it  is  dehydrated.  (Crookes, 
Phil.  Trans.  1910,  210.  A,  368.) 

+21H2O.    (Orlow,  Ch.  Z.  1912,  36.  1407.) 

Silver  platinocyanide,  Ag2Pt(CN)4. 
Insol.  in  H2O.    Sol.  in  NH4OH+Aq. 

Silver  platinocyanide  ammonia,  Ag2Pt(CN)4, 

2NH3. 
Insol.  in  H2O.     Sol.  in  NH4OH+Aq. 

Silver  platinocyanide  bromide. 
See  Bromoplatinocyanide,  silver. 

Silver  platinocyanide  chloride. 
See  Chloroplatinocyanide,  silver. 

Silver  platinocyanide  iodide. 
See  lodplatinocyanide,  silver. 

Sodium  platinocyanide,  Na2Pt(CN)4+3H2O. 
Easily  sol.  in  H2O.     (Willm,  Z.  anorg.  4. 

298.) 

Sol.  in  alcohol. 

Strontium  platinocyanide,  SrPt(CN)4+5H2O. 
Sol.  in  H2O. 

Thallous  platinocyanide,  Tl2Pt(CN)4. 

Nearly  insol.  in  cold,  si.  sol.  in  hot  H2O. 
(Friswell,  Chem.  Soc.  24.  461.) 

Thallous  platinocyanide  carbonate, 

2Tl2Pt(CN)4,  T12C03. 
Nearly  insol.  in  cold  H2O.    (F.) 

Thorium    platinocyanide,    Th[Pt(CN)4]2+ 

16H2O. 

Somewhat  difficultly  sol.  in  cold,  easily  in 
hot  H2O.  (Cleve,  Sv.  V.  A.  H.  Bih.  2.  No.  6.) 

Uranyl  platinocyanide,  (UO2)Pt(CN)4+a;H2O. 
Sol.  in  H2O.    (Levy,  Chem.  Soc.  1908,  93. 
1459.) 

Ytterbium  platuiocyanide,  2Yb(CN)3, 

3Pt(CN)2  +  18H2O. 

Easily  sol.  in  H2O.  (Cleve,  Z.  anorg.  1902, 
32.  139.) 

Yttrium    platuiocyanide,    Y2[Pt(CN)J3  + 

21H2O. 

Easily  sol.  in  H2O.  Insol.  in  absolute 
alcohol.  (Cleve  and  Hoglund.) 


Zinc   platinocyanide    ammonia,    ZnPt(CN)4, 
2NH3+H2O. 

Platinonitrous  acid. 

See  Platonitrous  acid. 

Platinoplatinicyanhydric  acid,  HPt(CN)4 

+zH20. 

Sol.  in  H2O.  (Levy,  Chem.  Soc.  1912,  101. 
1093.) 

Platinoselenocyanhydric  acid. 

Potassium  platinoselenocyanide, 

K2Pt(SeCN)6. 

Sol.  in  H2O  and  alcohol.  (Clarke  and  Dud- 
ley, B.  1878, 11.  1325.) 

Platinoselenostannic  acid. 

See  under  Selenostannate,  platinum. 

Platinososulphocyanhydric  acid, 

H2Pt(SCN)4. 
Known  only  in  aqueous  solution. 

Potassium  platinososulphocyanide, 

K2Pt(SCN)4. 

Permanent.  Sol.  in  2.5  pts.  H2O  at  15°, 
and  more  readily  at  higher  temp.  Very  sol. 
in  warm  alcohol. 

Silver ,  Ag2Pt(SCN)4. 

Insol.  in  H2O.  Sol.  in  KSCN+Aq,  and 
partly  sol.  in  NH4OH+Aq. 

Platinosulphocyanhydric  acid, 

H2Pt(SCN)6. 

Known  only  in  aqueous,  and  alcoholic  solu- 
tions. 

Ammonium  platinosulphocyanide, 

(NH4)2Pt(SCN)6. 
Sol.  in  H2O  and  alcohol. 

Barium ,  BaPt(SCN)6. 

Sol.  in  H2O  and  alcohol. 

Ferrous ,  FePt(SCN)6. 

Insol.  in  H2O  or  alcohol.  Not  attacked  by 
dil.  H2SO4,  HC1,  orHNO3+Aq. 

Lead  — ,  PbPt(SCN)6. 

SI.  sol.  in  cold,  decomp.  by  hot  H2O.  Sol. 
in  alcohol. 

PbPt(SCN)6,  PbO.  Insol.  in  H2O  or  alco- 
hol. Sol.  in  acetic  or  nitric  acids. 

Mercurous ,  Hg2Pt(SCN)6. 

Ppt.    Insol.  in  H2O. 


PLATINUM  AMMONIUM  COMPOUNDS 


731 


Potassium  platinosulphocyanide, 

K2Pt(SCN)6. 

Sol.  in  12  pts.  H2O  at  60°.  Much  more 
easily  in  boiling  H2O,  and  still  more  easily  in 
hot  alcohol. 

+2EUO.  (Miolati  and  Bellucci,  Gazz. 
Ch.  it.  1900,  30,  II.  592.) 

Silver  — ,  Ag2Pt(SCN)6. 

Insol.  in  H2O  or  K2Pt(SCN)6+Aq.  Sol. 
in  cold  NH4OH+Aq  and  in  KCNS+Aq. 

Sodium  — ,  Na;Pt(SCN)6. 
Sol.  in  H2O  and  alcohol. 

Platinosulphostannic  acid. 

See  under  Sulphostannate,  platinum. 

Platino sulphurous  acid. 

See  Plato  sulphurous  acid. 

Platinum,  Ft. 

Not  attacked  by  H2O,  H2SO4,  HC1,  or 
HNO3+Aq.  Slowly  sol.  in  aqua  regia,  or  a 
mixture  of  HBr  and  HNO3,  but  much  less 
easily  than  Au. 

Precipitated  Pt  is  remarkably  sol.  in 
HCl+Aq  in  presence  of  air.  (Wilm,  B.  1881, 
14.  636.) 

Pure  Pt  foil  is  attacked  by  fuming  HC1 
under  influence  of  light,  but  not  in  the  dark. 
(Berthelot,  C.  R.  1904,  138.  1297.) 

Dil.  HCl+Aq  dissolves  10-15%  Pt  from 
active  Pt  black.  (Wohler,  B.  1903,  36.  3482.) 

Cone.  HNO3  oxidizes  Pt  black;  Pt  sponge, 
less  easily;  sheet  Pt,  slightly.  (Wohler, 
Dissert.  1901.) 

Pt  in  presence  of  Hg  is  more  or  less  sol. 
in  cone.  HNO3.  (Tarugi,  Gazz.  ch.  it.  1903, 
33,  II.  171.) 

Pt  vessels  are  attacked  by  evaporating 
HNO3  therein.  (Jaunek  and  Meyer,  Z. 
anorg.  1913,  83.  71.) 

SI.  sol.  in  cone.  H2SO4  containing  small 
amounts  cf  nitrogen  oxides.  (Scheurer- 
Kestner,  C.  R.  86.  1082.) 

Pt  black,  pptd.  by  formic  acid,  is  easily 
sol.  in  boiling  H2SO4.  (Deville  and  Stas, 
Paris,  1878.) 

Thin  sheet  Pt  is  attacked  by  boiling  H2SO4 
containing  K2SO4;  1  sq.  cm.  loses  0.01  g. 
in  1  hour  and  velocity  of  the  reaction  is  not 
accelerated  by  addition  of  HNO3.  Pt  black 
is  completely  dissolved  under  the  above  con- 
ditions in  50  hours.  (Delepine,  C.  R.  1905, 
141.  1013.) 

Further  data  on  solubility  of  Pt  in  H2SO4 
are  given  by  Delepine.  (C.  R.  1906,  142. 
631.) 

95%  H2SO4  dissolves  0.04  g.  Pt  from  com- 
mercial Pt  at  250-260°  in  28  hours.  (Con- 
roy,  J.  Soc.  Chem.  Ind.  1903,  22.  465.) 

See  also  Quenessen.  (Bull  Soc.  1906, 
(3)  35.  620.) 


0.0038  g.  is  dissolved  by  10  cc.  of  boiling 
H2SO4.  (McCoy,  Eighth  Inter.  Cong.  App. 
Chem.  1912.  2.) 

HC1+HNO3,  so  long  as  they  are  sufficiently 
dil.  or  the  temperature  is  so  low  that  they 
cannot  react  on  each  other,  have  no  action  on 
Pt.  Addition  of  Cl  does  not  bring  about  re- 
action, but  a  few  drops  of  KNO2  or  N2O3+Aq 
bring  about  an  immediate  reaction.  (Millon.) 

Slowly  sol.  in  HI+Aq.  (Deville,  C.  R.  42. 
896.) 

Cone.  H3PO4  attacks  Pt  when  heated  in 
presence  of  air,  but  not  in  its  absence.  (Hiitt- 
ner,  Z.  anorg.  1908,  69.  216.) 

Pt  dissolves  easily  in  most  acids  when  they 
contain  H2O2.  (Fairley,  B.  1875,  8.  1600.) 

Slowly  sol.  in  boiling  FeCl3+Aq.  (Saint- 
Pierre,  C.  R.  64.  1077.) 

FeCl3  in  acid  solution  is  without  influence 
on  Pt.  (Marie,  C.  R.  1908,  146.  476.) 

Pt  is  completely  insol.  in  KCN+Aq. 
(Rossler,  Z.  Chem.  1866.  175.) 

Pt  is  attacked  by  boiling  cone.  KCN  +Aq. 
(Deville  and  Debray,  C.  R.  82.  241.) 

Solubility  of  Pt  in  10%  KCN+Aq  is  very 
small  at  ord.  temp.  (1.4  mg.  in  8  days)  but 
is  considerably  greater  in  boiling  cone.  KCN 
+Aq.  (71.5  mg.  in  5  hours).  (Glaser,  Z. 
Elektrochem.  1903,  9.  15.) 

Pt  foil  is  dissolved  in  boiling  KCN+Aq 
(0.030  g.  for  1  cc.  in  1  hour).  Insol.  in  cold 
KCN+Aq.  (Brochet  and  Petit,  C.  R.  1904, 
C.  R.  138.  1255.) 

Sol.  in  RbClJ+Aq.  (Erdmann,  Arch. 
Pharm.  1894,  232.  30.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 

Platinum  ammonium  compounds. 

Data  published  since  the  first  edition  of  this 
work  have  not  been  included  in  this  edition. 

See  — 


Platosamine  comps.,  Pt<i\rTr3  r> 

Platosem^'amine  comps., 
p,  .NH3.NH3.R 
Pt<R. 


Platowonoefo'amine  comps., 
NH3.NH3.R 


Platosamine  comps., 


NH3  NR3  R 


ine  comps.,  Pt<p     3 


Diplatocfo'amine  comps., 
Pt—  NH3.NH3.R 

Pt—  NH3.NH3.R 
Bromoplatinamine  comps., 


Chloroplatinamine  comps., 
NHs.R 
NH3.R. 


732 


PLATINUM  ANTIMONIDE 


Chloronitratoplatinamine  comps., 


topati 
- 


lodoplatinamine  comps., 

Hydroxyloplatinamine  comps. 
»TT\  TH^NH3.R 


Nitratoplatinamine  comps., 


Sulphatoplatinamine  comps., 


NH3.R. 

Bromoplatinse/ru'diamine  comps., 
Br3PtNH3.NH3.R. 

Bromonitritoplatinse  midiamine  comps.  , 
Br2(NO2)PtNH3.NH3.R. 

Chloroplatinsewzcfo'amine  comps., 
Cl3PtNH3.NH3.R. 

Chlorohydroxylonitritosemic^amine  comps.  , 
Cl(OH)(NO2)PtNH3.NH3.R. 

Chloronitritoplatinsemc&amine  comps., 
Cl2(NO2)PtNH3.NH3.R. 

lodoplatinseraicfaamine  comps., 
I3PtNH3.NH3.R. 

Hydroxylos  em  famine  comps., 
(OH)3PtNH3.NH3.R. 

Bromoplatinraonocfo'amine  comps., 

Rrp,  .NH3.NH3.R 
Br2Pt<NHsR 

Bromohydroxylopla  tin.monodiam.iae  comps. 
T}^r»T^T>f  ^NHs.NH.s.R 
Pt<NH3.R. 

Chloroplatinwonodiamine  comps., 
NH3.NH3.R 


lodonitratoplatinmonodiamine  comps., 

^Pt^NH3.NH3.R 
3)Pt<NH3R 

Hydroxyloplatinmono^'amine  comps., 

P^NH3.NH3.R 
2Pt<NHsR 

Bromoplatindzamine  comps., 
Rrp,     NH3.NH3.R 
lir2^t<NH3.NH3.R. 

Bromocarbonatoplatind^amine  comps., 


Bromochloroplatin^'amine  comps., 
BrClPt(NH3)4R2. 

Bromohydroxyloplatindzamine  comps., 
Br(OH)Pt(NH3)4R2. 

Bromonitratoplatindiamine  comps., 
Br(NO3)Pt(NH3)4R2. 

Bromosulphatoplatindmmine  comps., 
Br2(SO4)[Pt(NH3)4R2]2. 

Carbonatochloroplatindzamine  comps., 
(C03)Cl2[Pt(NH3)4R2]2. 

Carbonatonitratoplatindiamine  comps.  , 
(C03)(N03)2lPt(NH3)4R2]2. 


Chloroplatincfoamine  comps., 

:i2Pt(NH3)4R2. 

Chlorohydroxyloplatin^amine  comps., 
^1(OH)(NH3)4R2. 

Chloroiodoplatinrfiamine  comps., 
:iIPt(NH3)4R2. 

Chloronitratoplatindiamine  comps., 
Cl(NO3)Pt(NH3)4R2. 

Hydroxyloplatindiamine  comps., 
(OH)2Pt(NH3)4R2. 

Hydroxylonitratocfoamine  comps., 
(OH)(N03)Pt(NH3)4R2. 

Hydroxylosulphatodiamine  comps., 
(OH)2S04[Pt(NH3)4R2]2. 

lodoplatin^'amine  comps.,  I2Pt(NH3)4R2. 

lodonitritoplatindiamine  comps., 
I(N02)Pt(NH3)4R2. 

Nitratoplatindiamine  comps., 
(N03)2Pt(NH3)4R2. 

Nitritoplatincfo'amine  comps., 
(N02)2Pt(NH3)4R2. 

Sulphatoplatindiamine  comps., 
(S04)Pt(NH3)4R2. 

lodo^'platinamine  comps., 

T     pf<.NH3.R 
I— Pt<NHaR 

T  J>t.NH3.R 
Pt<NH3.R. 
Bromo^'platindiamine  comps., 


NH3.NH3.R 
NH3.NH3.R 


Br— Pt< 

R      L  .NH3.NH3.R 
Br~Pt<NH3.NH3.R. 

Hydroxylodiplatindiamine  comps., 
(OH)2Pt2(NH3)8R4. 

lodo^platin^amine  comps., 
I2Pt2(NH3)8R4. 

Nitratodiplatindiamine  comps., 
(N03)2Pt2(NH3)8R4. 

Platinfnamine  comps., 
P  p,  .NH3.NH3.NH3.R 
K2rt<NH3.NH3.NH3.R. 

77e^raplatinamine  comps.,  Pt4(NH3)8Rio. 

Octoplatinamine  comps.,  Pt8(NH3)i6Ri8. 

Platinum  antimonide,  PtSb2. 
(Christofie,  1863.) 

Platinum  arsenide,  Pt3As2. 
(Tivoli,  Gazz.  ch.  it.  14.  487.) 
PtAs2.     Min.  Sperrylite.     SI.  attacked  by 
aqua  regia.     (Wells,  Sill.  Am.  J.  (3)  37.  67.) 

Platinum  arsenic  hydroxide  (?),  PtAsOH. 

Insol.  in,  and  slowly  decomp.  by  H2O  and 
alcohol.  Easily  decomp.  by  HCl+Aq;  not 
attacked  by  HNO3+Aq.  Sol.  in  aqua  regia; 
not  attacked  by  cold  cone.  H2SO4,  but  de- 
comp. on  heating.  (Tivoli,  Gazz.  ch.  it.  14. 
487.) 


PLATINOUS  CHLORIDE  CARBONYL 


733 


Platinum  potassium  azoimide. 

Ppt.  Explodes  violently  even  in  aq.  solu- 
tion. (Curtius,  J.  pr.  1898,  (2)  68.  304.) 

Platinum  boride,  Pt2B2. 

Very  slowly  sol.  in  aqua  regia.  (Martins, 
A.  109.  79.) 

Platinous  bromide,  PtBr2. 

Insol.  in  H2O.  Sol.  in  HBr+Aq.  SI.  sol. 
in  KBr+Aq.  (Topsoe,  J.  B.  1868.  274.) 

Platinic  bromide,  PtBr4. 

Not  deliquescent;  sol.  in  H2O.  (Meyer 
and  Ziiblin,  B.  13.  404.) 

SI.  sol.  in  H2O.  100  g.  PtBr4+Aq  sat.  at 
20°  contain  0.41  g.  PtBr4.  (Halberstadt,  B. 
17.  2962.) 

Easily  sol.  in  HBr+Aq;  si.  sol.  in  HC2H3O2 
+Aq.  Sol.  in  considerable  amount  in  K  or 
NH4  oxalate+Aq. 

Very  si.  sol.  in  alcohol  or  ether,  also  in 
glycerine.  (Halberstadt.) 

Platinic  hydrogen  bromide. 
See  Bromoplatinic  acid. 

Platinous  bromide  carbonyl. 
See  Carbonyl  platinous  bromide. 

Platinic  bromide  with  MBr. 
See  Bromoplatinate,  M. 

Platinum  carbide,  PtC2. 

Hot  aqua  regia  dissolves  out  nearly  all  the 
Pt.  (Zeise,  J.  pr.  20.  209.) 

Platinum  carbon  efo'sulphide,  PtCS2. 
See  Platinum  sulphocarbide. 

Platinum  monochloride,  PtCl+zH2O. 

Easily  sol.  in  HC1;  mod.  sol.  in  hot  dil. 
H2S04  without  decomp.  (Sonstadt,  Proc. 
Chem.  Soc.  1898,  14.  179.) 

Platinous  chloride,  PtCl2. 

Insol.  in  H2O,  cone.  H2SO4,  or  HNO3.  Sol. 
in  hot  HCl+Aq  with  exclusion  of  air.  (Ber- 
zelius.) 

Insol.  in  alcohol  or  ether;  sol.  in  NH4OH  + 
Aq.  (Raewsky,  A.  ch.  (3)  22.  280.)  Sol.  in 
aqua  regia  with  formation  of  PtCl4. 

Insol.  in  cold  cone.  KI+Aq,  but  sol.  when 
heated.  (Lassaigne,  A.  ch.  (2)  51.  117.) 

SI.  sol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 

Insol.  in  acetone.  (Fidmann,  C.  C.  1899, 
II.  1014.) 

Platinum  ^'chloride,  PtCl3. 

SI.  sol.  in  cold,  more  sol.  in  hot  H2O. 
Partially  hydrolyzed  by  boiling  with  H2O. 


Insol.  in  cold  cone.  HC1.  Sol.  in  hot  cone. 
HC1  with  decomp. 

Sol.  in  KI+Aq.  (Wohler,  B.  1909,  42. 
3961.) 

Platinic  chloride,  PtCl4. 

Not  deliquescent.  Very  sol.  in  H2O.  (Pul- 
linger,  Chem.  Soc.  61.  420.) 

Sp.  gr.  of  aqueous  solution  containing: 

5         10  15        20        25  %  PtCl4, 

1.046  1.097  1.153  1.214  1.285 

30        35        40        45         50  %  PtCl4. 
1.362  1.450  1.546  1.666  1.785 
(Precht,  Z.  anal.  18.  512.) 

Insol.  in  cone.  H2SO4.    (Dumas.) 

SI.  sol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 

Sol.  in  alcohol  and  ether;  sol.  in  anhydrous 
acetone.  (Zeise,  A.  33.  34.) 

Insol.  in  ether.  (Willstatter,  B.  1903,  36. 
1830.) 

SI.  sol.  in  methvl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4328.) 

+H2O.  Sol.  in  H2O.  (Gutbier  and  Hem- 
rich,  Z.  anorg.  1913,  81.  378.) 

+4H20.  Sol.  in  H2O.  (Pigeon,  C.  R. 
1891,  112.  792.) 

+5H2O.  Not  deliquescent.  Sol.  in  H2O  or 
HCl+Aq. 

Composition  is  probably  H2PtCl4O+4H2O. 
(Norton,  J.  pr.  110.  469.) 

+7H2O.    Sol.  in  H2O.    (Pigeon.) 

+8H2O.  (Blondel,  A.  Ch.  1905,  (8)  6. 
98.) 

Platinic  thallium  chloride,  Tl3Pt2Cl8H5O4. 

Ppt.;  insol.  in  H2O.  (Miolati,  Z.  anorg. 
1900,  22.  460.) 

Platinous  hydrogen  chloride. 
See  Chloroplatinous  acid. 

Platinic  hydrogen   chloride. 
See  Chloroplatinic  acid. 

Platinous  chloride  with  MCI. 
See  Chloroplatinite,  M. 

Platinic  chloride  with  MCI. 
See  Chloioplatinate,  M. 

Platinous  phosphorus  chloride. 

See  Phosphorus  platinous  chloride. 

Platinic  phosphorus  chloride. 
See  Phosphorus  platinic  chloride. 

Platinous  chloride  carbonyl. 

See  Carbonyl  platinous  chloride. 


734 


PLATINUM  CHLORIDE  HYDROXYLAMINE 


Platinum  chloride  hydroxylamine, 
Pt(NH2OH)2Cl2. 

Ppt.  Sol.  in  alcohol  and  in  ether.  De- 
comp.  in  aq.  solution. 

Pt(NH2OH)4Cl2.  Sol.  in  H2O.  (Uhlen- 
huth,  A.  1900,  311.  124.) 

Platinous  chloride  sulphocarbamide, 

PtCl2,  4CS(NH2)2. 

SI.  sol.  in  H2O;  very  sol.  in  hot  H2O; 
decomp.  si.  on  boiling.  (Kurnakow,  J.  pr. 
1894,  (2)  50.  483.) 

Platinum  chloroiodide,  PtCl2I2. 

Very  deliquescent.  (Kammerer,  A.  148. 
329.) 

PtClI3.  Insol:  in  H2O.  SI.  sol.  in  alcohol. 
Sol.  in  KOH+Aq,  from  which  it  is  pptd.  by 
H2SO4.  (Mather,  Sill.  Am.  J.  27.  257.) 

Platinum  chloronitride,  PtNCl. 
(Alexander,  C.  C.  1887.  1254.) 

Platinous  cyanide  with  MCN. 
See  Platinocyanide,  M. 

Platinous  fluoride,  PtF2f?). 

Insol.  in  H2O.     (Moissan,  A.  ch.  (6)   24. 

287.) 

Platinic  fluoride,  PtF4. 

Deliquescent.  Sol.  in  H2O  with  immediate 
decomp.  into  PtO4H4  and  HF.  (Moissan,  C. 
R.  109.  807.) 

Platinous  hydroxide,  PtO2H2. 

Sol.  in  HC1,  HBr,  and  H2SO3+Aa,  but 
not  in  other  oxygen  acids.  Decomp.  by 
boiling  KOH+Aq.  (Thomsen,  J.  pr.  (2)  16. 
344.) 

When  freshly  pptd,  is  insol.  in  dil.  HNO3 
and  H2SO4,  and  in  HC2H3O2;  sol.  in  cone. 
HNO3  and  H2SO4.  Very  sol.  in  H2SO3  and 
HC1.  After  drying,  is  insol.  in  cone.  HNO3 
and  H2SO4.  (Wohler,  Z.  anorg.  1904,  40. 
424.) 

Platinic  hydroxide,  Pt(OH)4. 

Easily  sol.  in  dil.  acids  and  in  NaOH+Aq. 
(Topsoe',  J.  B.  1870.  386.) 

Nearly  insol.  in  acetic  acid.     (Dobereiner.) 

Insol.  in  all  acids  except  cone.  HC1  and 
aqua' regia.  fWohler,  Z.  anorg.  1904,  40. 
438.) 

+H2O.  Ppt.   (Prost,  Bull.  Soc.  (2)  44.  256.) 

Insol.  in  2N-H2SO4  and  dil.  HNO3+Aq: 
mod.  sol.  in  cone.  HNO3,  H2SO4,  2N-HC1  and 
NaOH+Aq.  (Wohler.) 

+2H2O.  Easily  sol.  in  dil.  acids,  even 
acetic  acid,  and  in  NaOH+Aq.  (Topsoe.) 

Insol.  in  acetic  acid;  si.  sol.  in  2N-H2SO4 
and  HNO3;  easily  sol.  in  HC1,  and  NaOH+ 
Aq.  (Wohler.) 


Platinoplatinic  hydroxide,  Pt3O4,  9H2O. 
Ppt.     (Prost,  Bull.  Soc.  (2)  46.  156.) 
11H2O.     Ppt.     (Prost.) 


Platinum  hydroxylamine  comps. 

See— 

Plato^oxamine   comps.,    Pt(NH3O)4R2. 

Platosoxamine      comps.,     Pt(NH3O)2R2. 

Platosoxamine-amine  comps., 
Pt(NH3O)3NH3R2. 

Platinous  iodide,  PtI2. 

Insol.  in  H2O,  acids,  or  alcohol.  (Lassaigne, 
A.  ch.  (2)  51.  113.) 

Difficultly  sol.  in  Na2SO3+Aq.     (Topsoe.) 

Gradually  decomp.  by  hot  HI+Aq  of  1.038 
sp.  gr.,  also  by  hot  KI+Aq,  PtI4  being  dis- 
solved out  and  Pt  left  behind.  Not  attacked 
by  cone.  H2SO4,  HC1,  or  HNO3+Aq,  but 
gradually  decomp.  by  KOH  or  NaOH+Aq. 
(Lassaigne.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1889, 
II.  1014.) 

Platinic  iodide,  PtI4. 

Insol.  in  H2O.  Sol.  in  NaOH  or  Na2CO3+ 
Aq,  H2SO3,  or  Na2SO3+Aq.  Sol.  in  HI+Aq 
or  alkali  iodides  +Aq.  Sol.  in  alcohol,  with 
partial  decomp.  Not  attacked  by  acids. 
(Lassaigne,  A.  ch.  (2)  61.  122.) 

Very  sol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 

Sol.  in  alcohol.  (Belluci,  C.  C.  1902,  I. 
625.) 

Platinic  iodide  with  MI. 
See  lodoplatinate,  M. 

Platinum  nitride  chloride,  PtNCl. 
See  Platinum  chloronitride. 

Platinous  oxide,  PtO. 

Sol.  in  H2SO3+Aq.  Insol.  in  other  acids. 
(Dobereiner,  Pogg.  28.  183.) 

Sol.  in  cone.  H2SO4;  easily  in  cone.  HC1+ 
Aq.  (Storer's  Diet.) 

Very  si.  sol.  in  HCl+Aq.  SI.  sol.  in  aqua 
regia.  (Wohler,  B.  1903,  36.  3482.) 

Platinic  oxide,  PtO2. 

Insol.  in  acids,  even  aqua  regia.  (Wohler, 
Dissert,  1901.) 

Platinum  £noxide,  PtO3 

Unattacked  by  dil.  H2SO4,  HNO3  or  acetic 
acid  Sol.  with  decomp.  in  dil.  and  cone.  HC1, 
cone.  H2SO4  or  cone.  HNO3.  (Wohler,  B. 
1909,  42.  3329.) 

Platinum  sesgwioxide,  Pt2O3+zH2O. 

Insol.  in  dil.  sol.  in  cone.  H2SO4.  SI.  sol.  in 
hot  dil.  HNO3.  Sol.  in  HC1.  Sol.  in  cone. 
alkali  hydroxides  +Aq.  (Wohler,  B.  1909,  42. 
3964.) 


PLATINUM  TELLURIDE 


735 


+2H20.  Insol.  in  HNO3  and  H2SO4. 
Insol.  in  alkalies  +Aq,  also  cold  dil.  HCl+Aq. 
Sol.  in  aqua  regia.  (Dudley,  Am.  Ch.  J. 
1902,  28.  66.) 

+5H2O.  (Delepine,  Bull.  Soc.  1910,  (4) 
7.  103.) 

Platinoplatinic  oxide,  Pt3O4. 

Not  attacked  by  long  boiling  with  HC1, 
HNO3,  or  aqua  regia.  (Jorgensen,  J.  pr.  (2) 
16.  344.) 

Does  not  exist.  (Wohler,  Z.  anorg.  1904, 
40.  450.) 

Platinum  oxychloride,  3PtO,  PtCl2  (?). 

Sol.  in  HC1,  and  in  KOH+Aq.  (Kane, 
Phil.  Trans.  1842.  298.) 

PtCl2(OH)2  =  H2PtCl2O2.  (Jorgensen,  J. 
pr.  (2)  16.  345.) 

5Pt02,  2HC1+9H2O.  Insol.  in  cold  H2O; 
decomp.  on  boiling.  Slowly  sol.  in  HC1. 
(Blondel,  A.  ch,  1905,  (8)  6.  100.) 

Platinum  oxysulphide,  PtOS. 
See  Platinum  sulphydroxide. 

Platinum  phosphide,  PtP2. 

Insol.  in  HCl+Aq.  Sol.  in  aqua  regia. 
(Schrotter,  W.  A.  B.  1849.  303.) 

PtP2H2.  Insol.  in  H2O,  and  HCl+Aq. 
(Cavazzi,  Gazz.  ch.  it.  13.  324.) 

PtP.  Insol.  in  aqua  regia.  (Clark  and 
Joslin.) 

Pt2P.  Sol.  in  aqua  regia.  (Clark  and 
Joslin.) 

••Pt3P5.    Partially  sol.  in  aqua  regia.    (Clark 
and  Joslin,  C.  N  48.  385.) 

Attacked  very  slowly  by  aqua  regia. 
Rapidly  sol.  in  molten  alkalies.  (Granger, 
C.  N.  1898,  77.  229.) 

Completely  sol.  in  aqua  regia  if  the  action 
sufficiently  prolonged,  though  with  difficulty. 
(Granger,  C.  R.  1893,  123.  1285.) 

Platinum  cftselenide,  PtSe2. 

As  PtS2.  (Minozz;,  Chem.  Soc.  1909,  96. 
(2)  899.) 

Platinum  friselenide,  PtSe3. 

SI.  attacked  by  hot  cone.  HNO3;  not  at- 
tacked by  cold  cone.  HCl+Aq;  slowly  sol. 
in  aqua  regia  and  Cl2+Aq;  insol.  in  CS2. 

Platinum  silicide,  Pt2Si. 

Sol.  in  hot  aqua  regia.  (Vigouroux,  C.  R. 
1896,  123.  117.) 

Pt3Si2.    (Co^on,  C.  R.  94.  27.) 

Pt4Si3.  Slowly  decomp.  by  aqua  regia. 
(Guyard,  Bull.  Soc.  (2)  25.  511.) 

PtSi.  Insol.  in  HNO,,  H2SO4,  HF,  and  HC1. 
Completely  sol.  in  aqua  regia.  (Lebeau  and 
Novitzky,  C.  R.  1907,  145.  241.) 


Platinum  sulphydroxide,  PtOS+H2O  = 

PtS(OH)2. 

Decomp.  easily  into — 
Pt2S203H2=^|  O  gg  =  PtOS  +  ^H20.  H20 

cannot  be  removed  without  decomposing  the 
compound,    (v.  Meyer,  J.  pr.  (2)  15.  1.) 

Platinous  sulphide,  PtS. 

Not  attacked  by  boiling  acids,  aqua  regia, 
or  KOH+Aq.  (BSttger,  J.  pr.  2.  274.) 

Sol.  in  large  excess  of  (NH4)2S+Aq. 

Platinoplatinic  sulphide,  Pt2S3. 

Not  attacked  by  HC1  or  HNO3+Aq,  and 
only  slowly  by  aqua  regia.  (Schneider,  Pogg. 
138.607.) 

Platinic  sulphide,  PtS2. 

Anhydrous.  Aqua  regia  attacks  si.,  other 
acids  not  at  all.  (Davy.) 

Hydrated  Insol.  in  HCl+Aq;  si.  sol.  in 
boiling  HNO3+Aq.  Sol.  n  aqua  regia. 
(Fresenius.)  Sol.  in  alkali  sulphides,  hydrates 
and  carbonates +Aq.  (Berzelius.)  Very  si. 
sol.  in  (NH4)2S+Aq.  (Claus.) 

Insol.  in  NH4C1,  or  NH4NO3+Aq. 

1  pt.  PtCl4  in  100  pts.  H  O+25  pts.  HC1  is 
not  pptd.  by  H2S.  (Reinsch.) 

Difficultly  sol.  in  alkali  sulphydroxides+ 
Aq,  but  more  easily  in  presence  of  SnS, 
Sb2S3,  As2S3,  or  SnS2.  (Ribau,  C.  R.  86. 
283.) 

Platinum  sulphide,  Pt6S6,  or    T^raplatinum 

sulphoplatinate,  4PtS,  PtS2. 
Decomp.  on  moist  air,  but  not  attacked  by 
acids.    (Schneider,  J.  pr.  (2)  7.  214.) 

Platinum  sulphides  with  M2S. 
See  Sulphoplatinate,  M. 

Platinum  sulphocarbide,  PtC2S2. 

Not  attacked  by  hot  HC1,  HN03+Aq, 
slightly  by  aqua  regia.  (Schiitzenberger, 
C.  R.  111.  391.) 

Platinum  teUuride,  PtTe. 

Decomp.  by  fused  oxidizing  agents;  slowly 
sol.  in  cone.  HNO3.  (Roessler,  Z.  anorg. 
1897,  15.  407.) 

Platinum  ditelluride,  PtTe2. 

Insol.  in  boiling  cone.  KOH+Aq;  slowly 
sol.  in  boiling  cone.  HNO3;  decomp.  oy  fused 
oxidizing  agents.  (Roessler.) 

Plato-. 

See  also  Plathio-. 


736 


PLATOAMIDOSULPHONIC  ACID 


Platoamidosulphonic  acid. 

Potassium  platoamidosulphonate, 

K2Pt(NH2S03)4+2H20. 
Very  si.  sol.  in  cold  H2O;  sol.  in  10  pts. 
boiling  H2O.      (Ramberg   and   St.   Kahlen- 
berg,  B.  1912,  46.  1514.) 

Sodium  ,  Na2(Pt(NH2S03)4+4H2O. 

Very  sol.  in  H26.  (Ramberg  and  St. 
Kahlenberg.) 

Platocframine  bromide,  Pt[(NH3)2Br]2  + 
3H2O. 

Easily  sol.  in  H2O.    (Cleve.) 

carbonate,  Pt(N2H6)2CO3+H2O. 

Sol.  in  H2O.    (Peyrone,  A.  61.  14.) 
Pt(N2H6Cp3H)2.    SI.  sol.  in,  but  decomp. 

by  boiling  with  H2O  into — 

sesgm'carbonate. 

More  sol.  than  preceding  salt.  (Reiset,  C. 
R.  11.  711.) 

chloride,  Pt[(NH3)2Cl]2+H20. 

"Reiset's  first  chloride."  Sol.  in  4  pts. 
H2O  at  16.5°,  and  in  less  hot  H2O.  Insol.  in 
alcohol  or  ether.  (Reiset,  A.  ch.  (3)  11.  419.) 

As  sol.  in  NH4Cl+Aq  as  in  H2O;  insol.  in 
absolute  alcohol;  si.  sol.  in  dil.  alcohol;  very 
sol.  in  dil.  HCl+Aq.  (Peyrone,  A.  ch.  (3)  12. 
19o.) 

cuprous  chloride,  Pt(NH3)4Cl2,  Cu2Cl2. 

Sol.  in  H2O,  and  pptd.  from  H2O  solution 
by  alcohol.  (Buckton.) 

cupric  chloride,  Pt(NH3)4Cl2,  CuCl2. 

SI.  sol.  in  cold,  decomp.  by  hot  H2O  into 
Pt(NH3)4Cl2,  Cu2Cl2.  (Buckton,  Chem.  Soc. 
6.  218.) 

Nearly  insol.  in  H2O;  easily  sol.  in  warm 
HCl+Aq;  insol.  in  alcohol.  (Millon  and 
Commaille,  C.  R.  67.  822.) 

Millon   and   Commaille's   salt   is 
Cu(NH3)4Cl2,  PtCl2,  cuprammonium  chloro- 
platinite. 

lead  chloride,  Pt(NH3)4Cl2,  PbCl2. 

Sol.  in  hot,  much  less  in  cold  H2O.  Insol. 
in  HCl+Aq  or  alcohol.  (Buckton,  Chem. 
Soc.  6. 213.) 

mercuric  chloride,  Pt(NH3)4Cl2,  HgCl2. 

Easily  sol.  in  hot  H2O,  much  less  in  cold. 
Insol.  in  HCl+Aq.  (Buckton.) 

zinc  chloride,  Pt(NH3)4Cl2,  ZnCl2. 

Easily  sol.  in  hot  H2O.  Insol.  in  alcohol. 
(Buckton.) 


Plato^amine    chloroplatinate,   Pt(NH3)4Cl2, 

PtCl4. 

Ppt.  Inso].  in  H2O.  (Cossa,  Gazz.  ch.  it. 
17.  1.) 

—  chloroplatinite,  Pt(NH3)4Cl2,  PtCl2. 
(Magnus'  green  salt.)    Insol.  in,  and  not  de- 
comp. by  H2O,  HCl+Aq,  or  alcohol.    (Mag- 
nus.) 

Slowly  sol.  in  boiling  NH4OH+Aq  and  in 
cone.  NH4  salts +Aq.  (Reiset,  A.  ch.  (3)  11. 
427.) 

Almost  as  sol.  in  (NH4)2CO3+Aq  as  in 
NH4OH+Aq.  Sol.  in  hot  PtCl4+Aq.  (Rei- 
set.) 

Not  decomp.  by  boiling  KOH,  dil.  HC1,  or 
H2SO4+Aq,  but  easily  by  HNO3+Aq. 
(Gros,  A.  27.  245.) 

chromate,  Pt(NH3)4CrO4. 

Scarcely  sol.  in  H2O.    (Cleve.) 

bichromate,  Pt(NH3)4Cr2O7. 

SI.  sol.  in  H2O.  Insol.  in  alcohol.  Sol.  in 
KOH+Aq.  (Buckton,  Chem.  Soc.  6.  213.) 

platinous  cyanide,  Pt(NH3)4(CN)2, 

Pt(CN)2. 

SI.  sol.  in  cold,  easily  in  boiling  H2O;  sol. 
in  KOH,  HC1,  and  dil.  H2SO,+Aq  without 
decomp.,  but  cone.  H2SO4  decomposes. 

potassium  ferrocyanide, 

Pt(NH3)4K2[Fe(CN)6]2+3H20. 

—  hydroxide,  Pt[(NH3)2OH]2. 

" Reiset's  first  base."  Easily  sol.  in  H2O. 
SI.  sol.  in  alcohol. 

— '—  iodide,  Pt[(NH3)2I2]. 

SI.  sol.  in  cold,  more  easily  in  hot  H2O,  but 
slowly  decomp.  on  boiling.  (Reiset.) 

—  nitrate,  Pt[(NH3)2NO3]2. 

Sol.  in  about  10  pts.  boiling  H2O.  Insol.  or 
but  si.  sol.  in  alcohol.  (Peyrone,  A.  ch.  (3) 
12.  203.) 

nitrate    sulphate,    [Pt(NH3)4NO3]2SO4, 

Pt(NH3)4S04. 

Very  easily  sol.  in  H2O.  (Carlgren,  Sv.  V. 
A.  F.  47.  310.) 


nitrite,  Pt[(NH3)2NO2]2+2H2O. 


Efflorescent.  Very  sol.  in  hot  or  cold  H2O. 
Insol.  in  90%  alcohol.  (Lang.) 

platinous  nitrite,  Pt[(NH3)2NO2]2, 

Pt(N02)2. 

Scarcely  sol.  in  cold,  somewhat  more  easily 
in  hot  H2O.  Not  attacked  by  cold  dil.  acids. 
More  sol.  in  NH4OH+Aq  than  in  H2O. 
(Lang.) 


PLATOAMINE  SULPHATE 


737 


Plataftamine     phosphate,     Pt(N2H6)2HPO4 

+H20. 

Rather  difficultly  sol.  in  cold,   and  very 
easily  in  hot  H2O.    (Cleve.) 

ammonium  phosphate, 

Pt[(N2H6)PO4(NH4)2]2,     4NH4H2PO4+ 
H2O. 

Very  easily  sol.  in  H2O  with  decomp.  into— 
Pt(N2H6H2PO4)2,  2NH4H2PO4+9H2O. 
Much  more  sol.  in  H2O  than  the  preceding, 
comp.  (Cleve.) 

sulphate,  Pt(NH3)4SO4. 

Sol.  in  32  pts.  H2O  at  16.5°;  more  easily 
when  heated .    ( Reiset . ) 

Sol.  in  50-60  pts.  boiling  H2O;  less  in  cold 


ing 
(Clc 


H2O;  insol.  in  alcohol.    (Cleve.) 

sulphate,  acid,  Pt[(NH3)2SO4H]2+H2O. 

Decomp.  by  H2O  or  alcohol  into  neutral 
salt. 

3Pt(NH3)4SO4,  H2SO4+H2O.  Sol.  in  H2O. 
(Cleve.) 

—  sulphite,  Pt(NH3)4SO3. 

Nearly  insol.  in  cold  H2O.    (Birnbaum,  A. 


152.  143.) 

Pt[(NH3)2S03H]2+2H20. 
HCl+Aq.    (Cleve.) 


Ppt.      Sol.    in 


— • — •  platinous  sulphite, 

3Pt(NH3)4SO3,  PtSO3+2H2O. 
Scarcely  sol.  in  cold  H2O;  sol.  in  190  pts. 

H2O  at  100°.    Easily  sol.  in  warm  HCl+Aq 

with  decomp.     (Peyrone.) 

+4H2O.    (Carlgren,  Sv.  V.  A.  F.  47.  308.) 
2Pt(NH3)4SO3,     PtSO3,  H2SO3     Insol.  in 

cold  H2O  or  alcohol.    Scarcely  sol.  in  hot  H2O. 

(Peyrone.) 

—  sulphocyanide,  Pt(NH3)4(CNS)2+H2O. 
Very  sol.  in  H2O.    Solution  is  decomp.  on 
boiling.    (Cleve,  Sv.  V.  A.  H.  10,  9.  7.) 


—  —  •  platinous  sulphocyanide, 

Pt(NH3)4(CNS)2,  Pt(CNS)2. 
Insol.  in  H2O  and  alcohol;  sol.  in  dil.  HC1+ 
Aq.     (Buckton,  Chem.  Soc.  13.  122.) 


Platowumodiamine  chloride,  Pt 

Easily  sol.  in  H2O.    (Cleve.) 

Pla.tomonodiam.ine  chloroplatinite 
2P  (NH3)2C1  ptri 
2Pt  '  PtUz' 


NH,Cl 

Moderately  sol.  in  cold,  but  more  easily  in 
hotH2O.    (Cleve.) 


nitrate, 
Easily  sol.  in  H2O.     (Cleve.) 


PUtoroonoeKamine  sulphate, 

Easily  sol.  in  cold,  but  much  more  in  hot 
H2O. 

Platosemiaiamine  bromide, 

Sol.  in  H2O.    Easily  sol.  in  NH4OH+Aq. 

(Cleve.) 

-  chloride,  Pt<g[H°)*C1 

(Peyrone's  chloride.)  Sol.  in  387  pts.*H2O 
at  0°,  and  26  pts.  at  100°  (Cleve);  in  33  pts.  at 
100°.  (Peyrone.) 

Sol.  in  NH4OH+Aq;  very  si.  sol.  in  HC1  or 
H2SO4+Aq;  more  easily  in  HNO3+Aq;  sol. 
in  alkali  carbonates  +Aq.  (Peyrone,  A.  ch. 
(3)  12.  193.) 

Plato  semidisLwme  chlorosulphurous  acid, 
p,  .(NH3)2S03H 
Pt<Cl. 
Easily  sol.  in  H2O.    (Cleve.) 

Ammonium  plaiosemidiamine  chlorosulphite 

pla.tosemidiam.ine  sulphite, 
p      (NH3)2S03NH4,  p      (NH3)2S03NH4  , 
Ft<Cl  Pt<S03NH4 

2H2O. 

Easily  sol.  in  H2O.     Insol.  in  alcohol. 
(Cleve.) 

Platosewi'cfa'amine  cyanide, 

Pt(CN)(NH3)2CN. 
Easily  sol.  in  H2O.    (Cleve.) 

-  platinous    cyanide,    Pt(CN)(NH3)2CN, 

Pt(CN)2(?). 
Ppt. 


hydroxide, 

Not  known. 


iodide, 
SI.  sol.  in  boiling  H,O.    (Cleve.) 

—  nitrate  PtgJ£->'NO' 

Moderately  sol.  in  H2O.    (Cleve.) 


-  nitrite, 

Very  si.  sol.  in  cold,  more  easily  in  hot  H2O. 

—  oxalate,  Pt(NH3)2C2O4. 
(Cleve.) 
+2H2O.    (Cleve.) 

-  sulphate,  Pt<(NH3)2>ga 

Very  si.  sol.  even  in  hot  H2O.    (Cleve.) 


738 


PLATOAMINE  SULPHOCYANIDE 


Platosemirfiamine  sulphocyanide, 

Pt(SCN)(NH3)2SCN. 

Easily  sol.  in  warm  H2O,  but  solution  soon 
decomposes. 

PlatosewiVfa'amine  sulphurous  acid. 

Ammonium  platoseraicftamine  sulphite, 
Pt<(NH3)2S03(NH4)   rNHNSO 
Ft<S03(NH4)  '  (NH4)2b03. 

Very  sol.  in  H2O.    (Cleve.) 

Barium ,  Pt(SO3)[(NH3)2SO3]Ba,  BaSO3. 

Ppt.    (Cleve.) 

Silver .   Pt(S03Ag)[(NH3)2S03Ag], 

Ag2S03. 
Ppt.     (Cleve.) 

Diplatocfo'amine  chloride,  Pt2(NH3)4Cl2. 
Insol.  in  H2O. 

hydroxide,  Pt2(NH3)4(OH)2+H2O. 

Insol.  in  H2O. 

—  nitrate,  Pt2(NH3)4(NO3)2. 
Insol.  in  H2O.    (Cleve.) 

sulphate,  Pt2(NH3)4SO4. 

Insol.  in  H2O.    (Cleve.) 

Platobromonitrous  acid. 

Potassium  platobromonitrite,  K2Pt(NO2)3Br 
+2H20. 

Sol.  in  about  3  pts.  cold,  and  2  pts.  boiling 
H2O.  (Vezes,  A.  ch.  (6)  29.  194.) 

K2Pt(NO2)2Br2-fH2O.  Sol.  in  1  pt.  cold, 
and  still  less  hot  H2O.  Insol.  in  alcohol. 


Platochloronitrous  acid. 

Potassium  chloronitrite,  K2Pt(NO2)sCl  + 
2H2O. 

Sol.  in  about  3  pts.  cold,  and  2  pts.  boiling 
H2O.    (Vezes,  A.  ch.  (6)  29.  178.) 

K2Pt(NO2)2Cl2.    Sol.  in  about  3  pts.  cold, 
and  2  pts.  boiling  H2O.     (Vezes.) 

Platochlorosulphurous  acid. 
See  Chloroplatosulphurous  acid. 

Platoiodonitrous  acid,  H2Pt(NO2)2I2. 

Known  only  in  solution.    (Nilson,  J.  pr.  (2) 
21.  172.) 

Aluminum  platoiodonitrite,   Al2[Pt(NO2)2I2]3 

+27H20. 
Easily  sol.  in  H2O.    (Nilson.) 

Ammonium—,  (NH4)2Pt(NO2)2I2+2H2O. 
Sol.  in  H2O;  decomp.  on  heating. 


Barium      platoiodonitrite,     BaPt(NO2)2Io 

4H2O. 
Very  sol.  in  H2O. 

Cadmium  -  ,  CdPt(NO2)2I2+2H2O. 
Easily  sol.  in  H2O. 

Caesium  -  ,  Cs2Pt(NO2)2I2+2H2O. 
Easily  sol.  in  H2O. 

Calcium—,    CaPt(NO2)2I2+6H2O. 
Very  easily  sol.  in  H2O. 

Cerium  -  ,  Ce2[Pt(NO2)2I2]3  +  18H2O. 
Easily  sol.  in  H2O. 

Cobalt—,  CoPt(NO2)2I2+8H2O. 
Sol.  in  H2O. 

Didymium  —  ,  Di2[Pt(NO2)2I2]3+24H2O. 
Sol.  in  H2O. 


Erbium  -  ,  Er2[Pt(NO2)2I2 
Sol.  in  H2O. 


H2O. 


Ferrous  —  ,  FePt(NO2)2I2+8H2O. 
Sol.inH2O. 

Ferric  -  ,  Fe2[Pt(NO2)2I2]3+6H2O. 
Sol.  in  H2O. 

Lanthanum  -  ,    La2[Pt(NO2)2I2]3+24H2O. 
Sol.  in  H2O. 

Lead  —  ,  basic,  PbPt(NO2)2I2,  Pb(OH)2. 
Insol.  in  H2O. 

Lithium  -  -,     Li2Pt(NO2)2I2+6H2O. 
Very  sol.  in  H2O. 

Magnesium  —  -,     MgPt(NO2)2I2+8H2O. 
Sol.  in  H2O. 

Manganese  -  ,  MnPt(NO2)2I2+8H2O. 
Sol.  in  H2O. 


Mercurous 


Hg20+9H26, 
Insol.  in  H2O. 


basic,    2Hg2Pt(NO2)2I2, 


Nickel ,  NiPt(NO?)2I2+8H2O. 

Sol.inH2O. 

Potassium—,  K2Pt(NO2)2I2+2H2O. 
Sol.  hi  H2O  in  all  proportions. 
Very  sol.  hi  alcohol. 

Rubidium—,   Rb2Pt(NO2)2I2+2H2O. 
i    Sol.  inH2O. 


PLATONITRITE,  POTASSIUM 


739 


Silver  platoiodonitrite,  Ag2Pt(NO2)2l2. 
Insol.  in  H2O. 

Sodium  -  ,  Na2Pt(NO2)2I2+4H2O. 
Very  sal.  in  H2O. 

Strontium  -  ,  SrPt(NO2)2I2+8H2O. 
Sol.  in  H2O. 

Thallium  --  -,  Tl2Pt(NO2)2I2. 
Insol.  in  H2O. 

Yttrium  —  ,  Y2[Pt(NO2)2I2]3+27H2O. 
Sol.  in  H2O. 

Zinc  --  -,  ZnPt(N02)2I2+8H2O. 
Sol.  in  H2O. 

Tn'platoocfonitrosylic  acid,  H4Pt3O(NO2)8. 
(Nilson,  J.  pr.  (2)  16.  241.) 

Potassium  ^nplatooctonitrosylate. 
See  under  Platonitrite,  potassium. 

Platonitrous  acid,  H2Pt(NO2)4. 

Sol.  in  H2O  or  alcohol.  (Lang.  J.  pr.  83. 
419.) 

Is  called  "  Platotefranitrosylic  acid"  by 
Nilson. 

Aluminum    platonitrite,    Al2[Pt(NO2)4]3  + 
14H2O. 

Sol.  in  H2O. 

Al2(OH)2[Pt(NO2)2]4O2  +  10H2O.  SI.  sol. 
in  cold,  easily  in  hot  H2O  and  alcohol.  (Nil- 
son,  B.  9.  1727.) 

Ammonium    platonitrite,    (NH4)2Pt(NO2)4+ 
2H20. 

Moderately  sol.  in  cold  H20.  (Nilson,  B. 
9.  1724.) 

Barium  platonitrite,  BaPt(NO2)4+3H2O. 

SI.  sol.  in  cold,   very  sol.  in  hot  H2O. 
(Lang.) 

Cadmium  platonitrite,  CdPt(N02)4+3H2O. 
Easily  sol.  in  H2O.    (Nilson.) 

Caesium  platonitrite,  Cs2Pt(NO2)4. 
Resembles  K  salt. 

Calcium  platonitrite,   CaPt(NO2)4+5H2O. 
Very  sol.  in  H2O.    (Nilson.) 


Cerium  platonitrite,  Ce2[Pt(NO2)4]3 
Sol.  inH2O.    (Nilson.) 

Chiomium  diplatonitrite, 

€r2(OH)2[Pt(NO2)2]4O2+24H2O. 
"  Sol.  inH2O.    (Nilson.) 


Cobalt  platonitrite,  CoPt(NO2)4+8H2O. 
Easily  sol.  in  H2O.    (Nilson.) 

Copper  platonitrite,  CuPt(NO2)4+3H2O. 

Sol.  in  H2O.    (Nilson.) 

3CuPt(NO2)4,  CuO  +  18H2O.  Decomp.  by 
H2O.  (Nilson.) 

Didymium    platonitrite,    Di2[Pt(NO2)4]3-f- 

18H20. 
Deliquescent;  sol.  in  H2O. 

Erbium  platonitrite,  Er2[Pt(NO2)4]3+9,  and 

21H20. 
Deliquescent:  sol.  in  H2O. 

Glucinum    diplatonitrite,     GlrPt(NO2)2]2O-h 

9H2O. 
SI.  sol.  in  cold  H2O. 

Indium  ^platonitrite,    In(OH)2[Pt(NO2)2]4O2 

+  10H2O. 
SI.  sol.  in  H2O. 

Fenic     ^'platonitrite,     Fe2[Pt(NO2)2]6O3  + 

30H2O. 
SI.  sol.  in  cold,  easily  in  hot  H2O. 

Lanthanum    platonitrite,    La2[Pt(NO2)4]3  + 

18H2O. 
Deliquescent;  sol.  in  H2O. 

Lead  platonitrite,  PbPt(NO2)4+3H2O. 
SI.  sol.  in  H2O.    (Nilson.) 

Lithium  platonitrite,  Li2Pt(NO2)4+3H2O. 
SI.  deliquescent;  easily  sol.  in  H2O. 

Magnesium  platonitrite,  MgPt(NO2)4+5H2O. 
Easily  sol.  in  H2O. 

Manganese     platonitrite,     MnPt(NO2)4+ 

8H2O. 
Sol.  in  H2O. 

Mercurous  platonitrite,  Hg2Pt(NO2)4,  Hg2O? 
Nearly  insol.  in  H2O.  (Lang,  J.  pr.  83.  415.) 
+H26.  Nearly  insol.  in  H2O.  (Nilson.) 

Nickel  platonitrite,  NiPt(NO2)4+8H2O. 
Easily  sol.  in  H2O.    (Nilson.) 

Potassium  platonitrite,  K2Pt(NO2)4. 

Sol.  in  27  pts.  H2O  at  15°;  more  easily  sol. 
in  warm  H2O.  (Lang,  J.  pr.  83.  415.) 

+2H2O.    Efflorescent.    (Lang.) 

K2H4Pt3O(NO2)6+3H2O.  Very  si.  sol.  in 
cold  (0.01  mol.  in  1 1.  at  16°),  but  very  easily 
in  hot  H2O.  (Vezes,  A.  ch.  (6)  29.  162.) 

K4Pt3O(NO2)8+2H2O.  SI.  sol.  in  warm 
H2O.  (Nilson.) 


740 


PLATONITRITE,  POTASSIUM,  BROMIDE 


Potassium  platonitrite  bromide. 

See  Platibromonitrite  and  platobromoni- 
trite,  potassium. 

Potassium  platonitrite  chloride. 
See  Plati-  and  platochloronitrite,  potassium. 

Potassium  plat  nitrite  hydrogen  chloride. 

K2Pt(N02)4,  HC1. 

Sol.  in  H2O.  (Miolati,  Att.  Line.  Rend. 
1896,  (5)  6,  II.  358.) 

Potassium  platonitrite  iodide. 

See  Plati-  and  platoiodonitrite,  potassium. 

Potassium  platonitrite  nitrogen  dioxide, 

K,PtrNOi)4>  2NO2. 

Violently  decomp.  by  H20.  (Miolati, 
Atti  Line.  Rend.  1896,  (5)  6,  II,  356.) 

Rubidium   platonitrite,   Rb2(Pt)(NO2)4,   and 

+2H20. 

Very  slowly  sol.  in  cold,  more  easily  in 
warm  H2O.  (Nilson.) 

Silver  platonitrite,  Ag2Pt(NO2)4. 
Very  si.  sol.  in  cold,  easily  in  hot  H2O. 

Silver  ^platonitrite,  Ag2Pt2(NO2)4O. 
Insol.  in  H2O.    (Nilson.) 

Sodium  platonitrite,  Na2Pt(N02)4. 
Easily  sol.  in  H2O. 

Strontium  platonitrite,  SrPt(NO2)4+3H2O. 

Somewhat  si.  sol.  in  cold  H2O,  but  easily 
sol.  in  warm  H2O. 

Thallium  platonitrite,  Tl2Pt(NO2)4. 
Very  si.  sol.  in  H2O.    (Nilson.) 

Yttrium    platonitrite,    Y2[Pt(NO2)J3+9,    or 

21H20. 
Sol.  in  H2O. 

Zinc  platonitrite,  ZnPt(NO2)4+8H2O. 
Sol.  in  H20. 

Plato  d /examine  chloride, 

Pt(NH3O.NH3OCl)2. 

Easily  sol.  in  H2O.  (Alexander,  A.  246. 
239.) 

chloroplatinite,    Pt(NH3O.NH3OCl)2, 

PtCl2. 

Sol.  in  warm  HCl+Aq.  Insol.  in  cold  H2O 
or  alcohol;  very  si.  sol.  in  hot  H2O.  (Alex- 
ander.) 

hydroxide,     Pt(NH3O.NH3O)2(OH)2. 

Insol.  in  B2O  or  alcohol.  Easily  sol.  in  HC1 
or  HNO3+Aq.  Difficultly  sol.  in  hot  dil. 
H2SO4+Aq.  (Alexander.) 


Platodioxamine  oxalate, 

Pt(NH3O.NH3O)2C2O4. 
Insol.  in  cold  H2O,  alcohol,  or  organic  acids. 
(Alexander.). 

—  phosphate,  Pt3(NH3O.NH3O)12(PO4)2-f 

3H2O. 
Ppt.    (Alexander.) 

sulphate,  Pt(NH3O.NH3O)SO4+H2O. 

SI.  sol.  in  H2O.    (Alexander,) 

Platosamine  bromide,  Pt(NH3Br)2. 
SI.  sol.  even  in  hot  H2O.    (Cleve.) 

— -  chloride,  Pt(NH3Cl)2. 

"  Reiset's  second  chloride."  Sol.  in  1 40  pts. 
H2O  at  100°.  (Peyrone,  A.  61.  ISO.) 

Sol.  in  130  pts.  H2O  at  100°,  and  4472  pts. 
atO°.  (Cleve.) 

Easily  sol.  in  NH4OH+Aq,  HNO3,  or  aqua 
regia,  with  decomp.  Sol.  in  KClSl  -j-Aqfwith 
evolution  of  NH3.  (Cleve.) 

•  ammonium   chloride,   Pt(NH3Cl)2, 

2NH4C1. 

SI.  sol.  in  cold,  easily  in  hot  H2O;  insol.  in 
alcohol;  sol.  in  NH4OH  or  (NH4)2CO3+Aq. 
(Grimm,  A.  99.  75.)  * 

Platosamine  chlorosulphurous  acid, 

p,NH3Cl 

rtNH3SO3H. 

Easily    sol.    in    H2O    without    decomp. 
(Cleve.) 

Ammonium  platosamine  chlorosulphite, 

Pt(NH3Cl)NH3SO3NH4+H2O. 
Sol.  in  H2O.     (Peyrone,  A.  61.  180.) 

Platosamine  cyanide,  Pt(NH3CN)2. 

Quite  easily  sol.  in  H2O  or  NH4OH+Aq. 
(Buckton.) 

hydroxide,  Pt(NH3OH)2. 

"Reiset's  second  base."  Very  sol.  in  H2O. 
(Odling,  B.  3.  685.) 

iodide,  Pt(NH3I)2. 

Very  si.  sol.  in  H2O.  Sol.  in  cold  NH4OH+ 
Aq  to  form  platodiamine  iodide.  (Cleve.) 

nitrate,  Pt(NH3NO3)2. 

Moderately  sol.  in  hot  H2O.  Sol.  in 
NH4OH+Aq  with  combination.  (Reiset,  A. 
ch.  (3)  11. 26.) 

nitrite,  Pt(NH3NO2)2. 

Very  si.  sol.  in  cold,  easily  in  hot  H2O. 
Insol.  in  alcohol.  (Lang.) 


PLATOSULPHITE,  POTASSIUM 


741 


Platosamine  platinous  nitrite,  Pt(NH3NO2) 

Pt(N02)2. 

Slowly  and  si.  sol.  in  cold,  more  easily  sol.  in 
hot  H2O. 

Extremely  si.  sol.  even  in  cone,  acids;  more 
sol.  in  NH4OH+Aq  than  in  H2O.  (Lang.) 

—  oxide,  Pt(NH3)2O. 

Insol.  in  H2O  or  NH4OH+Aq.     (Reiset.) 

—  oxalate,    Pt(NH3)2H2(C2O4)2+2H2O. 
Ppt.     (Cleve.) 

—  sulphate,  Pt(NH3)2SO4+H2O. 

SI.  sol.  in  cold,  more  easily  in  hot  H2O. 

sulphite,  Pt(NH3)2SO3+H2O. 

Easily  sol.  in  H2O.    (Cleve.) 

sulphocyanide,  Pt(NH3SCN)2. 

Insol.  in  H2O;  can  be  cryst.  from  alcohol; 
not  attacked  by  HC1  or  H2SO4+Aq.  (Buck- 
ton.) 

Very  sol.  in  hot  H2O.    (Cleve.) 

silver  sulphocyanide, 

Pt(NH3)2Ag4(SCN)6. 
(Cleve.) 

Platosamine  sulphurous  acid, 

Pt(NH3S03H)2. 
Exists  only  in  its  salts. 
See  Platosamine  sulphite. 

Ammonium  platosamine  sulphite, 

Pt(NH3SO3NH4)2. 
Sol.  in  H2O.    Insol.  in  alcohol. 

Barium  platosamine  sulphite, 

Pt(NH3)2(S03)2Ba+3H20. 
Ppt.    (Cleve.) 

Cobalt  —    — 
6H20. 


Pt(NH3)2(S03)2CO  + 


Very  si.  sol.  in  H2O.     Sol.  in  HCl+Aq. 


Copper    - 
5H2O. 


,     Pt(NH3)2(SO3)2Cu  + 

Very  si.  sol.  in  H2O;  sol.  in  HCl+Aq. 

,  Pt(NH3)2(S03)2Pb+H20. 


Lead- 
Ppt. 


Manganese  — 
+4H20. 
Ppt.    SI.  sol.  in  H2O. 


,    Pt(NH£)2(SO3)?Mn 


Nickel 


-,  Pt(NH3)2(S03)2Ni+7H20. 


SI.  sol.  in  H2O. 


Sodium  platosamine  sulphite, 

Pt(NH3SO3Na)2+5^H2O. 
Sol.  in  H2O.    100  com.  sat.  solution  at  20° 
contains  5.52  g.  cryst.  salt.     (Haberland  and 
Hanekop,  A.  246.  235.) 


Silver 
Ppt. 


-,  Pt(NH3S03Ag)2+H20. 


Uranyl  --  —  ,  Pt(NH3)2(SO3)2UO2+H2O. 
Ppt. 

Zinc  --  ,  Pt(NH8)2(SO3)2Zn+6H2O. 
Ppt.    Very  si.  sol.  in  H2O.    (Cleve.) 

Platososermamine  potassium  chloride, 
PtQ11'01,  KC1+H20. 

Very  sol.  in  H2O;  insol.  in  alcohol.    (Cossa, 
B.  23.  2507.) 

Platosoxamine  chloride,  Pt 


Sol.  in  H2O.  Much  less  sol.  in  H2O  than 
platoeftoxamine  chloride.  (Alexander,  A. 
246.  239.) 

Platosoxamine  amine  chloride, 


Easily  sol.  in  H2O.     Insol.  in  alcohol  and 
cone.  HCl+Aq.     (Alexander,  A.  246.  239.) 


-  chloroplatinite, 

Ppt. 

Platosulphurous  acid. 


Ammonium  platosulphite,  (NH4)6Pt(SO3)4  + 

3H2O. 

Sol.  in  H2O.    (Birnbaum,  A.  139.  170.) 
(NH4)2Pt(SO3)2+H2O.    Sol.inH2O.    (Lie- 
big,  Pogg.  17.  108.) 

Ammonium  platosulphite  chloride, 
(NH4)2Pt(S03)2,  2NH4C1.  • 

Sol.  in  H2O.     (Birnbaum.) 

PtClSO3H,  2NH4C1.  Deliquescent;  sol.  in 
H2O.  (Birnbaum,  A.  162.  143.) 

See    also  Chloroplatosulphite,  ammonium. 

Potassium  platosulphite,  K6Pt(SO3)4+4H2O. 

SI.  sol.  in  cold,  easily  in  hot  H2O.  Much 
more  sol.  than  the  Na  salt.  (Birnbaum,  A. 
139.  168.) 

+3H2O.    (Lang,  J.  pr.  83.  415.) 

6K2O,  2PtO,   10SO2.     SI.  sol.  in  H2O. 
Glaus,  J.  B.  1847-48.  453.) 

Does  not  exist.    (Lang.) 

K2Pt(SO3)2.     Sol.  in  H2O. 


742 


PLATOSULPHITE,  SILVER 


Silver  platosulpbite,  Ag6Pt(SO3)4. 

Ppt.  Very  sol.  in  cold  NH4OH+Aq. 
(Lang.  J,  pr.  83.  415.) 

Sodium  platosulphite,  Na6Pt(SO3)4. 

Very  si.  sol.  in  cold,  somewhat  more  easily 
in  hot  H2O.  Not  decomp.  by  boiling  KOH  or 
NaOH+Aq.  Gradually  sol.  in  (NH4)2S  or 
K2S+Aq.  Insol.  in  NaCl+Aq  or  alcohol. 
(Litton  and  Schnedermann,  A,  42.  316.) 


+7H2O. 

Na2Pt(SO3H)4.  Moderately  sol.  in  H20. 
(Litton  and  Schnedermann.) 

Platothiosulphuric  acid. 

Sodium  platothiosulphate,  Na6Pt(S2O3)4+ 
10H2O. 

Very  sol.  in  H2O  (Schottlander,  A.  140. 
200.) 

PtS2O3,  4Na2S2O3  +  10H2O. 

PtS2O3,  6Na2S2O3  +  19H2O. 

2Pt2S2O3,  7Na2S2O3  +  18H2O.  (Jochum, 
C.  C.  1885.  642.) 

Plumbic  acid. 

Barium  plumbate,  Ba2PbO4. 

Insol.  in  H2O.  Sol.  in  HCl+Aq  with 
evolution  of  Cl.  Sol.  in  acids  in  presence  of  a 
reducing  substance.  (Kassner,  Arch.  Pharm. 
228.  109.) 

Calcium  plumbate. 

Insol.  in  H2O.  HNO3+Aq  dissolves  out 
CaO.  (Crum,  A.  65.  218.) 

Ca2PbO4.  Properties  as  Ba2PbO4.  (Kass- 
ner, Arch.  Pharm.  228.  109.) 

+4H2O.  Easily  decomp.  by  HNO3. 
(Kassner,  Arch.  Pharm.  1894,  232.  378.) 

Calcium  hydrogen  plumbate,  H2CaPb2O6. 

Fairly  stable;  slowly  sol.  in  HNO3  in  the 
cold.  (Kassner.) 

Calcium  lead  or//ioplumbate,  CaPbPbO4. 

Insol.  in  H2O.  Sol.  in  HC1.  HNO3,  acetic 
and  other  acids  cause  a  separation  of  PbO2. 
(Kassner,  Arch.  Pharm.  1903,  241.  147.) 

Copper  raetaplumbate,  CuPbO3. 

Decomp.  by  acids.  Insol.  in  NH4OH+Aq. 
Acetic  acid  dissolves  Cu.  (Hoehnel,  Arch. 
Pharm.  1896,  234.  399.) 

Lead  raetaplumbate,  PbPbO3. 

Identical  with  lead  sesquioxide.  (Hoehnel, 
Arch.  Pharm.  1896,  234.  399.) 

Manganese  metoplumbate. 

Decomp.  by  acids.  (Hoehnel,  Arch.  Pharm. 
1896,  234.  399.) 


Potassium  plumbate,  K2PbO3+3H2O. 

Very  deliquescent.  Decomp.  by  pure  H2O 
into  PbO2  and  KOH.  Sol.  in  KOH  + Aq  with- 
out decomp.  (Fremy,  J.  Pharm.  (3)  3.  32.) 

Silver  metoplumbate,  Ag2PbO3. 

Ppt.  (Griitzner,  Arch.  Pharm.  1895,  233. 
518.) 

Sodium  plumbate. 

Sol.  in  H2O  with  decomposition.  SI.  sol.  in 
alkalies +Aq.  (Fremy,  A.  ch.  (3)  12.  490.) 

Sodium  metaplumbate,  Na2PbO3+4H2O. 

Decomp.  by  H2O;  insol.  in  alcohol.  (Hoeh- 
nel, Arch.  Pharm.  1894,  232.  224.) 

Strontium  plumbate,  Sr2PbO4. 

Properties  as  Ba2PbO4.  (Kassner,  Arch. 
Pharm.  228.  109.) 

Zinc  wetoplumbate,  ZnPbO3+2H2O. 

Decomp.  by  dil.  acids;  insol.  in  H2O. 
(Hoehnel,  Arch.  Pharm.  1896,  234.  398.) 

Plumb  ous  acid. 

Calcium  plumbite. 

SI.  sol.  in  H2O.    (Karsten,  Scher.  J.  5.  575.) 

Potassium  plumbite,  PbO,  zK2O. 
Known  only  in  solution. 

Silver  plumbite,  Ag2PbO2. 

Insol,  in  H20,  NH4OH+Aq  and  KOH+ 
Aq;  sol.  in  HNX)3  and  acetic  acid;  and  in  cone. 
H2SO4,  HI,  and  HF.  (Bullnheimer,  B.  1898, 
31.  1288.) 

+2H2O.  Insol.  in  H2O.  Decomp.  on  air. 
(Kratwig,  B.  15.  264.) 

Sodium  plumbite. 

Known  only  in  solution. 

Potassium,  K2. 

Violently  decomposes  H2O  or  alcohol. 
Insol.  in  hydrocarbons.  Sol.  with  violent 
action  in  acids. 

Solubility  in  fused  KOH  at  t°. 


t° 

G.  K  sol.  in  100  g.  fused  KOH 

480 
600 
650 
700 

7.8-8.9 
3     -4 
2     -2.7 
0.5-1.3 

(Hevesy,  Z.  Elektmchem.  1909,  15.  534.) 

Sol.  in  liquid  NH3.    (Seely,  C.  N.  23.  169); 
(Franklin,  Am.  Ch.  J.  1898,  20.  829.) 

1  gram  atom  of  K  dissolves  in  4.74  mol. 


POTASSIUM  ARSENIDE,  AMMONIA 


743 


liquid  NH3  at  0°;  in  4.79  mol.  at  —50°;  in 
4.82  mol.  at  —100°.  (Ruff,  B.  1906,  39.  839.) 

Insol.  in  liquid  CO2.  (Biichner,  Z.  phys. 
Ch.  1906,  54.  674.) 

Slowly  sol  in  ethylene  diamine.  Insol.  in 
ethyl  amine  and  in  secondary  and  tertiary 
amines.  (Kraus,  J.  Am.  Chem.  Soc.  1907, 
29.  1561.) 

Potassium  acetylide,  K2C2. 

(Moissan,  C.  R.  1898,  127.  917.) 

Potassium  acetylide  acetylene,  K2C2,  C2H2. 
(Moissan,  C.  R.  1898,  127.  915.) 

Potassium  amalgams. 

Hg4K,  Hg5K,  HgK,  Hg10K,  Hg12K  and 
Hg]8K.  (Guntz,  C.  R.  1900,  131.  183.) 

Hgi4K.  Stable  up  to  0°.  Can  be  cryst. 
from  Hg  without  decomp.  below  0°. 

Hg12K.  Stable  from  0°  to  71°  or  73°.  Can 
be  cryst.  from  Hg  without  decomp.  at  any 
temp,  between  these  limits. 

Hg10K.  Stable  from  71°  or  73-75°.  Can 
be  cryst.  from  Hg  without  decomp.  at  any 
temp,  between  these  limits.  (Kerp,  Z.  anorg. 
1900,  25.  68.) 

Potassium  amide,  KH2N. 

Decomp.  by  water  or  alcohol.  Insol.  in 
hydrocarbons. 

Potassium  ammonickelate,  Ni2N3K5,  6NH3. 

Decomp.  by  H2O.  SI.  sol.  in  liquid  NH3. 
(Bohart,  J.  phys.  Chem.  1915,  19.  559.) 

Potassium  ammonoargentate,  AgNHK,  NH3 

or  AgNH2,  KNH2. 

Ppt.,  decomp.  in  the  air.  Decomp.  by  H2O 
or  by  liquid  NH3  solutions  of  acids.  (Frank- 
lin, J.  Am.  Chem.  Soc.  1915,  37.  855.) 

Potassium  ammonobarate,  BaNK,  2NH3. 

Hydrolyzed  by  H2O.  Insol.  in  liquid  NH3. 
Decomp.  and  dissolved  in  a  solution  of 
NH4NO3  in  liquid  NH3.  (Franklin,  J.  Am. 
Chem.  Soc.  1915,  37.  2297.) 

Potassium     ammonocadmiate,     Cd(NHK)2, 
2NH3. 

Ppt.    (Franklin,  Am.  Ch.  J.  1912,  47.  310.) 
Cd(NHK)2,    2NH3.      Decomp.    by    H2O. 

Insol.  in  liquid  NH3.    (Bohart,  J.  phys.  Chem. 

1915,  19.  542.) 

Potassium  ammonocalciate,  CaNK,  2NH3. 

Hydrolyzed  by  H2O.  Readily  sol.  in  a 
solution  of  NH4NO3  in  liquid  NH3.  (Frank- 
lin, J.  Am.  Chem.  Soc.  1915,  37.  2300.) 

Potassium  ammonocuprite,  CuNK2,  3NH3. 
Very  sol.  in  liquid  NH3. 
CuNK2,  2NH3. 


CuNK2,  NH3.  (Franklin,  J.  Am.  Chem. 
Soc.  1912,  34.  1503.) 

CuNK2,  2>iNH3,  Ppt.  (Franklin,  Am. 
Ch.  J.  1912,  47.  311.) 

Potassium  ammonomagnesate,  Mg(NHK)2. 

2NH3. 

SI.  sol.  in  liquid  NH3.  Rapidly  hydrolyzed 
by  H2O.  (Franklin,  J.  Am.  Chem.  Soc.  1913, 
35.  1463.) 


Potassium  ammonoplumbite,  PbNK, 

Completely  hydrolyzed  by  action  of  water 
vapor.  Violently  decomp.  by  H2O  or  dil. 
acids.  Sol.  in  liquid  NH3.  (Franklin,  J. 
phys.  Chem.  1911,  15.  519.) 

Potassium  ammonostannate,  Sn(NK)2,  4NH8. 
Decomp.  by  H2O.  Readily  sol.  in  HC1+ 
Aq.  SI.  sol.  in  liquid  NH3.  Readily  sol.  in  a 
solution  of  NH4I  in  liquid  NH3.  (Fitzgerald, 
J.  Am.  Chem.  Soc.  1907,  29.  1696.) 

Potassium  ammonostrontiate,  SrNK,  2NH3. 
Hydrolyzed  vigorously  by  H2O.     Sol.  in 
solutions  of  NH4NO3  in  liquid  NH3.     Insol. 
in  liquid  NH3.    (Franklin,  J.  Am.  Chem.  Soc. 
1915,  37.  2299.) 

Potassium  ammonotballate,  T1NK2,  4NH3. 

Sensitive  to  action  of  air  or  moisture.  Vio- 
lently decomp.  by  H2O  or  dil.  acids.  Mod- 
erately sol.  in  liquid  NH3  at  20°,  more  sol. 
at  higher  temp,  and  much  less  sol.  at  lower 
temp.  Decomp.  by  liquid  NH3  solutions  of 
acids.  (Franklin,  J.  phys.  Chem.  1912,  16. 
689.) 

Potassium  ammonotitanate,  (N)  TiNHK. 

Vigorously  hydrolyzed  by  H2O.  Insol.  in 
liquid  NH3  solutions  of  either  potassium 
amide  or  NH4Br.  (Franklin,  J.  Am.  Chem. 
Soc.  1912,  34.  1500.) 

Potassium  ammonozincate,  Zn(NHK)2, 
2NH8. 

Decomp.  by  water.  SI.  sol.  in  liquid  NH8. 
(Fitzgerald,  J.  Am.  Chem.  Soc.  1907,  29.  663.) 

Decomp.  by  H2O.  Sol.  in  dilute  acids. 
SI.  sol,  in  liquid  NH8.  Sol.  in  solutions  of 
ammonium  salts  in  liquid  NH«.  (Franklin, 
Z.  anorg.  1907,  55.  195.) 

Potassium  arsenide,  K3As. 
(Hugot,  C.  R.  1899,  129.  604.) 
K2As4.    (Hugot.) 

Potassium  arsenide,  ammonia,  AsK3,  NH8. 
Nearly  insol.  in  liquid  NH3.    (Hugot.) 
K2As4,  NH3.    (Hugot.) 


744 


POTASSIUM  AZOIMIDE 


Potassium  azoimide,  K 
Stable  in  aq.  solutioi 
46.5  pts.  are  sol.  in 

at. 
i. 

100  pts.  H2O  at  10.5°. 
100    "  H2O     "  15.5. 
100    "  H2O     "  17. 
100    "  abs.  alcohol  at 

(Curtius,  J.  pr.  1898, 

Br. 
L  100  pts.  H2O  at  t°. 

41.5+0.1378t   from   30°    to    120°.      (fifcard. 
C.  R.  98.  1432.) 

Solubility  of  KBr  in  100  g.  H2O  at  t°. 

48.9     "     "      "     " 
49.6     "     "     "     " 
0.1375     "     "     "     " 
16°. 
Insol.  in  pure  ether. 
(2)  68.  280.) 

Potassium  bromide,  K 
Solubility  of  KBr  ic 

t 

G.  KBr. 

t 

G.  KBr. 

10.5 
10 
3.5 
0 
-5 
-8 

UK 

62.1 

60.7 
55.5 
52.6 
50.1 
47.5 
45.3 

-11 

-10.5 
-10 

-  8.5 
-  8 
-  6.5 

44.9 
41.8 
39.7 
35.7 
31.2 
25.0 

t° 

Pts.  KBr 

t° 

Pts.  KBr 

(Meusser,  Z.  anorg.  1905,  44.  80.) 

68.74  g.  KBr  are  sol.  in  100  g.  H2O  at  25°. 
(Amadori  and  Pampanini,  Rend.  Ac.  Line. 
1911,  V,  20.  473.) 

Sp.  gr.  of  KBr+Aq  at  19°. 

0 
20 
40 

53.48 
64.52 
74.63 

60 
80 
100 

85.35 
93.46 
102.0 

(Kremers,  Pogg.  97.  151.) 
Solubility  of  KBr  in  100  pts.  H2O  at  t°. 

t° 

Pts.  KBr 

t 

Pts.  KBr 

%KBr 

Sp.  gr. 

%KBr 

Sp.  gr. 

—13.4 
—  6.2 
0 
+3.4 
5.2 
12.65 
13.0 
13.3 
18.3 
26.05 
30.0 
37.9 

46.17 
49.57 
53.32 
55.60 
56.63 
61.03 
61.17 
61.45 
64.11 
68.31 
70.35 
74.46 

43.15 

45.45 
50.5 
54.8 
60.15 
66.75 
71.45 
74.85 
86.5 
97.9 
110.0 

77.0 

77.73 
80.33 

82.78 
85.37 
88.22 
90.69 
92.25 
97.28 
102.9 
110.3 

5 
10 
15 
20 
25 

1.037 
1.075 
1.116 
1.159 
1.207 

30 
35 

40 
45 

1.256 
1.309 
1.366 
1.432 

(Gerlach,  Z.  anal.  8.  285.) 

Sp.  gr.  of  KBr+Aq  at  15°  containing: 
5            10          20           30          36%  KBr. 
1.0357     1.074     1.1583     1.2553     1.3198 
(Kohlrausch,  W.  Ann.  1879.  1.) 

Sp.  gr  of  KBr+Aq  at  t°. 

Solubility  is  represented  by  a  straight  line 
of  the  formula  54.43  +0.5128t.     (Coppet,  A. 
ch.  (5)  30.  416.) 
100  pts.  KBr+Aq  sat.  at  15-16°  contain 
39.06  pts.  KBr.    (v.  Hauer,  J.  pr.  98.  137.) 

Solubility  of  KBr  in  100  pts.  H2O  at  high 
temp. 

G.  KBr  dis- 
solved in  100  g 
H2O 

G.  KBr  in  100 
g.  of  the                t° 
solution 

Sp.  gr. 

4.166 

11.111 

25.000 
42.867 

4 
10 
20 

30 

14.5 
15.7 
16.5 
16.0 

]  .  0291 
1  .  0753 
1.1625 
1.2580 

t° 

Pts.  KBr 

140 
181 

120.9 
145.6 

(de  Lannoy,  Z.  phys.  Ch.  1895,  18.  460.) 

(Tilden  and  Shenstone,  Phil.  Trans.  1884. 23.) 
Sat.  solution  boils  at  112°.    (Kremers.) 

Sat.  KBr+Aq  contains  at: 
—12°      —10°       +3°       32°        39° 
31.0         31.5        35.7       41.6      47.7%  KBr, 

55°  77°         140°       173°      220° 

45.5         48.7        54.1       58.5       61.6%  KBr. 
(fitard,  A.  ch.  1894,  (7)  2.  539.) 

If  solubility  S  =  pts.  KBr  in  ICO  pts.  solu- 
tion, S  =  34.5+0.2420t  from  0°  to  40°,  S  = 


gr.  20°/20°  =  1.0521.    (Le  Blanc  and  Rohland, 
Z.  phys.  Ch.  1896,  19.  278.) 

Sp.  gr.  of  KBr+Aq  at  20.5°. 


Normality  of 
KBr+Aq. 

G.  KBr  inlOO  g. 
of  solution 

Sp.  gr.  t°/4° 

4.29 

3.01 
2.00 
1.00 

37.97 
28.83 
20.49 
11.03 

1.3449 
1.2407 
1.1629 
1.0815 

(Oppenheimer,  Z.  phys.  Ch.  1898,  27.  452.) 


POTASSIUM  BROMIDE 


745 


Solubility  of  KBr+NH4Br  at  25°. 

Solubility  of  KBr+KCl  in  H2O  at  t°. 

%  KBr 

%  NH4Br 

Sp.  gr 

t 

Sat.  solution  contains 

55.81 
55.42 
53.65 
51.68 
44.12 
34.73 
26.23 
26.03 
23.22 
22.23 
17.99 
0.0 

0. 
0. 
2. 
5. 
15. 
26. 
34. 
38. 
41. 
43. 
48. 
57. 

0 
64 
46 
13 
29 
22 
76 
14 
78 
25 
08 
73 

1.3756 
1.3745 
1.3733 
1.3721 
1.3711 
1.3715 
1.3753 
1.3753 
1.3766 
1.3777 
1.3766 
1.3763 

%  KC1 

%  KBr 

%  total  salt 

-14 
-13.7 
-13.5 
-7 
+5.2 
+6 
10 
21 
26 
30 
32 
39 
47 
52 
55 
71 
73 
102 
152 
160 
168 
225 

10.7 
l6!  7 

ii!3 

11.0 
10.8 
11.2 

ii!6 
ii!6 

11.0 
11.9 
12.0 
11.8 
12.8 
13.2 
12.5 

li!7 

18.8 

19^8 

22^6 
23.7 

25.5 
26\6 

30"8 
31.2 
29.9 
31.7 
32.9 
35.8 
40.6 
42.3 

45^6 

29.5 
29.4 
29.5 
30.5 
34.4 
33.9 
34.7 
35.3 
36.7 
39.4 
38.5 
39.8 
41.8 
42.2 
41.8 
43.7 
44.7 
48.6 
53.8 
54.8 
55.0 
59.7 

(Fock,  Z.  Kryst.  Min.  1897,  28.  357.) 
Solubility  in  KNO3+Aq. 

1 

litre  of  the  solution  contains 

at  14.5° 

at  25.2° 

Mol.  KN03 

Mol.  KBr 

Mol.  KNO3 

Mol.  KBr 

0.0 
0.362 
0.706 
1.235 

4.332 

4.156 
4.093 
3.939 

0.0 

0.131 
0.527 
0.721 
1.090 
1.170 
1.504 

4.761 

4.72 
4.61 
4.54 
4.475 
4.44 
4.375 

(fitard,  A.  eh.  1894,  (7)  3.  281.) 
Solubility  of  KBr+KCl  in  H2O  at  25°. 

G.  per  100  g.  H2O. 

KBr 

KCl 

68.47 
62.26 
58.50 
52.45 
45.42 
38.70 
26.62 
12.94 
0.0 

0.0 
5.43 
8.46 
12.48 
17.17 
21.23 
25.88 
31.02 
36.12       • 

(Touren,  C.  R.  1900,  130.  911.) 
See  also  under  KNO3. 

100  pts.  KBr+KCl+Aq  sat.  at  15-16°  con- 
tain 37.55  pts.  of  the  two  salts;    10.0  pts. 
KBr+KI+Aq  sat.  at  15-16°  contain  57.96 
pts.  of  the  two  salts;  100  pts.  KBr+KCl  + 

KI+Aq  sat.  at  15-16°  contain  57.88  pts.  of 
the  three  salts,    (v.  Hauer,  J.  pr.  98.  137. 


(Amadori  and  Pampanini,  Att.  Ace.  Line. 
1911,  20,  II.  475.) 

Solubility  in  KCl+Aq  at  25.2°. 


ooaiDUity  01  j\.Br-r-iY<ji  in  ja2u  at  air. 

1  litre  of  the  solution  contains 

%  KBr 

%  KCl 

Sp.  gr. 

Mol.  KCl 

Mol.  KBr 

55.81 

0.00 

1.3756 

0.0 

4.761 

53.15 

2.34 

1.3700 

0.67 

4.22 

50.36 

4.66 

1.3648 

0.81 

4.15 

45.46 

8.26 

1.3544 

1.35 

3.70 

37.96 

13.66 

1.3320 

1.48 

3.54 

32.48 

16.69 

1.3119 

1.61 

3.42 

21.80 

21.39 

1.2689 

1.70 

3.34 

14.07 

25.09 

1.2455 

2.46 

2.50 

4.75 

29.17 

1.1977 

3.775 

0.525 

0  00 

31.13 

1    IT^fi 

\J  .  \J\J 

JL  .  J.  I  OU 

(Touren,  C.  R.  1900,  130.  1252.) 

(Fock,  Z.  Kryst.  Min.  1897,  28.  357.) 

See  also  under  KCl. 

746 


POTASSIUM  BROMIDE 


By  repeatedly  heating  KBr+Aq  sat.  at  15- 
16°  with  KI  and  cooling  to  15°,  nearly  all  the 
KBr  can  be  separated,  (v.  Hauer.) 

100  pts.  H2O  sat.  with  KBr  at  16°  dissolve 
13.15  pts.  KI,  but  on  addition  of  more  KI, 
KBr  is  pptd.  (van  Melckebeke,  C.  C.  1872^ 
586.) 

Solubility  in  KI+Aq  at  t°. 


t° 

Sat.  solution  contains 

%  KBr 

%KI 

%  total  salt 

-22 

8.3 

42.6 

50.9 

-19 

9.5 

42.8 

52.3 

-6 

9.3 

44.7 

54.0 

-1.5 

t 

55.3 

+3 

HK3 

45^9 

56.2 

13.6 

10.1 

46.2 

55.9 

25 

10.8 

48.0 

58.8 

44.2 

11.1 

50.1 

61.2 

51 

12.1 

50.0 

62.1 

66 

10.8 

53.1 

63.9 

70 

11.6 

51.9 

63.5 

80 

12.3 

52.5 

64.8 

.93 

13.0 

53.7 

66.7 

116 

13.2 

54.6 

67.8 

125 

13.7 

54.8 

68.5 

150 

15.1 

55.1 

70.2 

175 

16.0 

57.2 

73.2 

175 

.  .  . 

.  .  . 

72.7 

195 

16.7 

56.5 

73.2 

220 

17.6 

57.0 

74.6 

(Etard,  A.  ch.  1894,  (7)  3.  279.) 
Solubility  of  KBr+KI  in  H2O  at  25°. 


G.  per  100  g.  H2O. 


KBr 


53.21 
42.32 
34.14 
30.08 
29.62 
22.15 
21.88 
18.54 
0.0 


KCl 


35.92 

66.63 

95.36 

119.59 

119 

127.10 
127.31 
130.61 
149.26 


(Amadori  and  Pampanini,  Att.  Ace.  Line. 
1911,  20,  II.  475.) 

Solubility  of  KBr  in  KOH+Aq. 


G.  per  1000  g.  H2O 

G.  per  1000  g.  H2O 

KOH 

KBr 

KOH 

KBr 

36.4 
113.5 
177.2 
231  .  1 

558.4 
433.6 
358.1 

281:2~- 

277.6 
434.7 
579.6 
806.9 

248.1 
137.1 
64.8 
33.4 

(Ditte,  C.  R.  1897,  124.  30.) 


Sol.  in  Br2  at  15°.  (Walden,  Z.  anorg.  1900, 
25.  220.) 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  829.) 

Sol.  in  liquid  NH3.  45  pts.  are  sol.  in  100 
pts.  liquid  NH3  at  —50°.  (Joannis,  C.  R. 
1905,  140.  1244.) 

Attacked  bv  liquid  NO2  with  liberation  of 
Br2.  (Frankland,  Chem.  Soc.  1901,  79. 
1361.) 

Insol.  in  liquid  CO2.  (Biichner,  Z.  phys. 
Ch.  1906,  54.  674.) 

Sol.  in  SO3.  (Walden,  Z.  anorg.  1900,  25. 
217.) 

Sol.  in  SO2C1(OH).  (Walden,  Z.  anorg. 
1902,  29.  382.) 

Difficultly  sol.  in  AsBr8.  (Walden,  Z. 
anorg.  1902,  29.  374.) 

Sol.  in  SbCl3.  (Walden,  Z.  anorg.  1900,  25. 
220.) 

Sol.  in  liquid  SO2.  (Walden,  Z.  -anorg. 
1902,30.  160.) 

Hydrazine  dissolves  56.4  pts.  KBr  at  12.5- 
13°.  (de  Bruyn,  R.  t.  c.  1899,  18.  297.) 

SI.  sol.  in  alcohol.    (Ballard.) 

Sol.  in  200  pts.  cold,  and  16  pts.  boiling 
80%  alcohol. 

Sol.  in  180  pts.  90%  alcohol.    (Hager.) 

Sol.  in  750  pts.  abs.  alcohol  at  15°.  (Eder, 
Dingl.  221.  89.) 

100  pts.  absolute  methyl  alcohol  dissolve 
1.51  pts.  at  25°;  100  pts.  absolute  ethyl  al- 
cohol dissolve  0.13  pt.  at  25°.  (de  Bruyn,  Z. 
phys.  Ch.  10.  783.) 


Solubility  of  KBr  in  methyl  alcohol +Aq  at 
25°. 

p=  %  by  wt    Of  aicohol  in  alcohol +Aq. 
S=Sp.  gr.  of  alcohol +Aq  sat.  with  KBr. 
L=  mUlimols  KBr  in  100  ccm.  of  the  solu- 
tion. 


p 

S  25°/4° 

L 

0 

1.3797 

471 

10.6 

1.300 

389 

30.8. 

1.159 

252 

47.1 

1.058 

162 

64.0 

0.9801 

87 

78.1 

0.8906 

44 

98.9 

0.8411 

23 

100 

0.8047 

14.2 

(Herz  and  Anders,  Z.  anorg.  1907,  65.  273.) 


100  g.  KBr+CH3OH  contain  0.2  g.  KBr 
at  the  critical  temp.  (Centnerszwer,  Z.  phys. 
Ch  1910,72.437.) 


POTASSIUM  SELENIUM  BROMIDE 


747 


Solubility  of  KBr  in  ethyl  alcohol  +Aq. 

Solubility  of  KBr  in  acetone  +Aq  at  25°. 

Temp.  =30° 

Temp.  =40° 

KBr=  millimols   KBr   in    100   cc.    of   the 

wt.  % 

alcohol 

G.  KBr.  per  100  g. 

G.  KBr  per  100  g. 

solution. 

Solution 

Solvent 

Solution 

Solvent 

A 

KBr 

Sp.  gr. 

0 

41.62 

71.30 

43.40 

76.65 

0 

481.3 

1.3793 

5 

38.98 

67.25 

40.85 

72.70 

20 

366.7 

1.2688 

10 

36.33 

63.40 

38.37 

69.00 

30 

310.5 

1.2118 

20 

31.09 

56.40 

33.27 

62.30 

40 

259.0 

1  .  1558 

30 

25.98 

50.15 

28.32 

56.45 

50 

202.9 

1.0918 

40 

21.24 

44.95 

23.22 

50.46 

60 

144.9 

1  .  0275 

50 

16.27 

38.85 

18.11 

44.25 

70 

95.3 

0.9591 

60 

11.50 

32.50 

13.02 

37.40 

80 

46.5 

0.89415 

70  - 

6.90 

24,70- 

.  7.98  . 

28.90 

90 

10.1 

0.8340 

80 

3.09 

15  .  95 

3.65 

18.95 

90 

0.87 

8.80 

1.03 

10.45 

(Herz  and  Knoch,  Z.  anorg.  1905,  45.  262.) 

(Taylor,  J.  phys.  Ch.  1896, 1.  724.) 


At  room  temp.,  1  pt.  KBr  by  weight  is  sol. 
in: 
52  pts.  methyl  alcohol,  D15  0.7990. 
350    "    ethyl          "        D1£  0.8100. 
1818    "    propyl       "       D*5  0.8160 

(Rohland,  Z.  anorg.  1898,  18.  325.) 
Solubility  of  KBr  in  ethyl  alcohol  at  0°. 

Solubility  of  KBr  in  glycerine  +Aq  at  25°. 

G=g.  glycerine  in  100  g.  glycerine  +Aq. 
KBr=  millimols  KBr  in  100  cc.  of  the  solu- 
tion. 

G 

KBr 

Sp.  gr. 

0 
13.28 
25.98 
45.36 
54,23 
83.84 
100 

481.3 
444.3' 
404.0 
340.5 
310.4 
219.25 
172.65 

1.3793 
1.3704 
1.3655 
1.3594 
1.3580 
1.3603 
1.3691 

Cone,  of  alcohol 
in  mol.  g.  per  1. 
H20 

G.  KBr  in 
1  1.  H20 

Mol.  solubility 

1 
2 

536.75 
529.25 
502.85 
491.  15 
455.25 

4.51 
4.45 
4.22 
4.13 
3.82 

(Herz  and  Knoch,  Z.  anorg.  1905,  45.  267.) 

100  g.  95%  formic  acid  dissolve  23.2  g. 
KBr  at  18.5°.    (Aschan,  Chem.  Ztg.  1913,  37. 

(Armstrong  and  Eyre,  Proc.  R.  Soc.  1910, 

[A]  84.  127.) 


100  g.  methyl  alcohol  dissolve  2.17  g.  KBr 
at  25°, 

100  g.  ethyl  alcohol  dissolve  0.142  g.  KBr 
at  25°. 

100  g.  propyl  alcohol  dissolve  0.035  g  KBr 
at  25°. 

100  g.  isoamyl  alcohol  dissolve  0.003  g.  KBr 
at  25°. 

(Turner  and  Bissett,  Chem.  Soc.  1913,  103. 
1909.) 


0.055  g.  is  sol.  in  100  g.  propyl  alcohol. 
(Schlamp,  Z.  phys.  Ch.  1894,  14.  276.) 

Sol.  in  5000  pts.  ether  (sp.  gr.  0.729  at  15°.) 
(Eder,  L  c.) 

Sol.  in  1700  pts.  alcohol-ether  (1  :  1)  at  15° 
(Eder,  I.  c.) 

100  pts.  acetone  dissolve  0.023  pt.  KBr  at 
25°,  (Krug  and  M'Elroy,  J.  Anal.  Ch.  6. 184.) 


1117.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1904,  37.  3601.) 

Insol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1370.) 

100  ccm.  of  a  sat.  solution  of  KBr  in  fu?- 
furol  at  25°  contain  0.139  pts.  by  wt.  KBr. 
(Walden,  Z.  phys.  Ch.  1906,  55.  713.) 

Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.  257.) 

Potassium  rhodium  bromide. 
See  Bromorhodite,  potassium. 

Potassium  ruthenium  inbromide. 
See  Bromoruthenite,  potassium. 

Potassium  ruthenium  te/rabromide. 
See  Bromoruthenate,  potassium. 

Potassium  selenium  bromide. 
See  Bromoselenate,  potassium. 


748 


POTASSIUM  TELLURIUM  BROMIDE 


Potassium  tellurium  bromide. 
See  Bromotellurate,  potassium. 

Potassium  thallic  bromide,  KBr,  TlBr3+ 
2H2O. 

Sol.  in  H20. 

3KBr,2TlBr3+3H20.  SoUnH,O.  (Ram- 
melsberg.) 

Potassium  thorium  bromide. 
Sol.  inH2O.    (Berzelius.) 

Potassium    tin    (stannous)    bromide,    KBr, 

SnBr2+H20. 

Sol.  in  H2O.     (Benas,  C.  C.  1884.  958.) 
Can  be  recryst.  from  HBr  or  KBr+Aq. 

(Richardson,  Am.  Ch.  J.  14.  95.) 
2KBr,  SnBr2+2H2O.    Cannot  be  recryst. 

from  HBr+Aq.     (Richardson.) 

Potassium    tin    (stannic)    bromide,    2KBr, 

SnBr4. 
See  Bromostannate,  potassium. 

Potassium  uranous  bromide,  KUBr6. 

Very  sol.  in  H2O.  (Alov,  Bull.  Soc.  1899, 
(3)  21.  264.) 

Potassium  uranyl  bromide,  2KBr,  UO2Br2  + 

2H2O. 
Very  easily  sol.  in  H2O.    (Sendtner.) 

Potassium  zinc  bromide,  KBr,  ZnBr2+2H2O. 

Not  hygroscopic.  (Ephraim,  Z.  anorg. 
1908,  59.  60.) 

2KBr,  ZnBr2+2H2O.  Not  hygroscopic. 
(Ephraim.) 

Potassium  bromide  ammonia,  KBr,  4NH3. 
(Joannis,  C.  R.  1905,  140.  1244.) 

Potassium  bromide  ruthenium  dihydronitro- 
sochloride,  (NO)Ru2H2Cl3,  2HC1,  3KBr. 
Ppt.     SI.  sol.  in  H2O.     (Brizard,  A.  ch. 
1900,  (7)  21.  359.) 

Potassium  bromoiodide,  KBr2I. 

Decomp.  rapidly  on  air.  (Wells  and 
Wheeler,  Sill.  Am.  J.  143.  475.) 

Potassium  carbonyl,  K2C2O2. 

Decomp.  by  H2O  with  explosion.  (Joannis, 
C.  R.  116.  158.) 

Potassium  chloride,  KC1. 

Sol.  in  H2O  with  absorption  of  heat. 

30  pts.  KC1+100  pts.  H2O  at  13.2°  lower 
the  temp.  12.6°.  (Riidorff,  B.  2.  68.) 

100  pts.  H2O  dissolve  29.31  pts.  KC1  at  0°. 
(Gay-Lussac);  28.5  pts.  KC1  at  0°  (Mulder; 
Gerardin.) 


The  saturated  solution  contains  58.5%,  and 
boils  at  107.6° (Mulder);  contains59.40%,  and 
boils  at  108.3°  (Legrand);  contains  59.26%, 
and  boils  at  109.6°  (Gay-Lussac);  boils  at 
110°.  (Kremers.) 

Sol.  in  3.016  pts,  H2O  at  15°  (Gerlach);  in 
3.03  pts.  at  17.5°,  or  100  pts.  H2O  at  17.5°  dis- 
solve 33  pts  KC1.  (Schiff.) 

100  pts.  H2O  at  t°  dissolve  pts.  KC1: 


t° 

Pts. 
KC1 

t. 

Pts. 
KC1 

t° 

Pts. 
KC1 

59.26 

0 
19.35 

29.21 
34.53 

52.39 
79.58 

43.59 
50.93 

109.60 

(Gay-Lussac,  A.  ch.  (2)  11.  308.) 


100  pts.  H2O  dissolve  34.6  pts.  KC1  at  11.8°;  34.9 
pts.  at  J.3.80;  35  pts.  at  15.6°.  (Kopp.) 

100  pts.  H2O  at  17.5°  dissolve  33.24  pts.  KC1,  and 
sp.  gr.  of  solution  is  1.635.  (Karsten.) 

100  pts.  H20  at  12°  dissolve  32  pts.,  and  at  100°,  59.4 
pts.  (Otto -Graham.) 

Sol.  in  3  pts.  H2O  at  ord.  temp.,  and  3  pts.  boiling 
H2O  (Bergmann) ;  in  3.33  pts.  hot  or  cold  H2O  (Four- 
croy);  in  3  pts.  at  15°,  and  1.68  pts.  at  110°  (M.  R.  and 
P.) 

Sol.  in  3.5  pts.  H2O  at  0°,  and  in  less  than  1  pt.  hot 
H2O  (Schubarth);  100  pts.  H2O  at  17.5°  dissolve  30.7- 
33.0  pts.  KC1  (Ure's  Diet.). 

100  pts.  H2O  dissolve  35.405  .pts.  KC1  at  15°,  and 
solution  has  sp.  gr.  =1.1809.  (Michel  and  Krafft,  A. 
ch.  (3)  41.  478.) 


100  pts.  H2O  dissolve  at: 
18°      30°      40°      57° 
33.6    37.8    40.1     45.0  pts.  KC1. 
(Gerardin,  A.  ch.  (4)  5.  139.) 


100  pts.  H2O  dissolve  33.06-32.08  pts.  KC1 
at  15.6°  and  sp.  gr.  of  solution  =  1.171.  (Page 
and  Keightley,  Chem.  Soc.  (2)  10.  566.) 


Solubility  in  100  pts.  H2O  at  t°. 


t° 

Pts. 
KC1 

t° 

Pts. 
KC1 

t° 

Pts. 
KCl 

0 

28.5 

17 

33.9 

34 

38.5 

1 

28.7 

18 

34.2 

35 

38.7 

2 

29.0 

19 

34.4 

36 

39.0 

3 

29.3 

20 

34.7 

37 

39.3 

4 

29.5 

21 

35.0 

38 

39.6 

5 

30.0 

22 

35.3 

39 

39.9 

6 

30.5 

23 

35.5 

40 

40.1 

7 

31.0 

24 

35.8 

41 

40.3 

8 

31.5 

25 

36.1 

42 

40.6 

9 

31.7 

26 

36.4 

43 

40.9 

10 

32.0 

27 

36.6 

44 

41.2 

11 

32.3 

28 

36.9 

45 

41.5 

12 

32.5 

29 

37.2 

46 

41.7 

13 

32.8 

30 

37.4 

47 

42.0 

14 

33.1 

31 

37.7 

48 

42.3 

15 

33.4 

32 

38.0 

49 

42.5 

16 

33.6 

33 

38.2 

50 

42.8 

POTASSIUM  CHLORIDE 


749 


Solubility  in  100  pts.,  etc.—  Continued. 

If  solub] 

lity  S  =  pts.  KCl  in  100  pts.  solu- 
0.5+0.1445t  from  —90°  to   110°. 
R.  98.  1432.) 

1+Aq  contains  at: 
150°         175°         180° 
38.8         41.2         41.8%  KCl. 

200°        242°         732°  (mpt.) 
42.9         47.6          100%  KCl. 
rd,  A.  ch.  1894,  (7)  2.  256.) 

;2O  dissolve  0.488  gram-equivalent 
°.     (van't  Hoff  and  Meyerhoffer, 
h.  1904,  49.  315.) 

ibility  of  KCl  in  H2O  at  t°. 

t° 

Pts. 
KC1 

t° 

Pts. 
KCl 

t 

Pts. 
KCl 

(fitard,  C. 

Sat.  KG 
142° 
38.6 

190° 
43.2 

(fita 

100  g.  H 
KCl  at  25 
Z.  phys.  C 

Soh 

51 
52 
53 
54 
55 
56 
57 
58 
59 
60 
61 
62 
63 
64 
65 
66 
67 
68 
69 
70 

43.1 
43.4 
43.6 
43.9 
44.2 
44.4 
44.7 
44.9 
45.2 
45.5 
45.8 
46.1 
46.3 
46.6 
46.9 
47.2 
47.5 
47.7 
48.0 
48.3 

71 

72 
73 
74 
75 
76 
77 
78 
79 
80 
81 
82 
83 
84 
85 
86 
87 
88 
89 
90 

48.5 
48.8 
49.1 
49.4 
49.6 
49.9 
50.2 
50.5 
50.8 
51.0 
51.3 
51.5 
51.8 
52.1 
52.4 
52.6 
52.9 
53.2 
53.5 
53.8 

91 
92 
93 
94 
95 
96 
97 
98 
99 
100 
101 
102 
103 
104 
105 
106 
107 
107.65 

54.1 
54.4 
54.6 
54.9 
55.2 
55.5 
55.7 
56.0 
56.3 
56.6 
56.9 
57.2 
57.4 
57.7 
58.0 
58.2 
58.5 
58.5 

G. 

KCl  per 

100  G.  H2O. 

t° 

KCl 

Sp.  gr. 

0.70 
19.55 
32.80 
59.85 
74.80 
89.45 
108.0* 

28.29 
34.37 
38.32 
45.84 
49.58 
53.38 
58.11 

1.1540 
.1738 
.1839 
.1980 
.2032 
.2069 
.2118 

(Mulder,  calculated  from  his  own  and  other 
observations,  Scheik.  Verhandel.  1864.  41.) 

Solubility  in  100  pts.  H2O  at  t°. 

*  Bpt.  of  sat.  solution. 
(Berkeley,  Phil.  Trans.  Roy.  Soc.  1904,  203, 
A.  189.) 

Solubility  of  KCl  in  100  g.  H2O  at  t°. 

t° 

Pts. 
KCl 

t° 

Pts. 
KCl 

t° 

Pts. 
KCl 

-11° 
-6.4 

24.46 
25.78 
27.9 
29.37 
30.84 
32.19 
>  32.66 
34.32 

25.7 
29.25 
38.0 
41.45 
46.15 
48.8 
55.1 
60.55 

36.10 
37.31 
39.71 
40.67 
42.34 
42.86 
44.51 
45.90 

64.95 
71.65 
74.25 
80.75 
86.6 
91.4 

47.17 
48.76 
49.27 
51.24 
52.53 
53.49 

0 
+3.9 
9.4 
11.4 
14.  & 
19.0 

t° 

g- 

KCl 

t° 

g.  KCl 

+  18.5 
11.5 
10 
7.5 
2.5 
0 
-1 

33.3 
31.2 
30.8 
29.8 
28.4 
27.5 
27.2 

-4.5 
-9 

-8.5 
-8 

7'i 

25.9 
23.9 
21.5 
20.0 
17.5 
15.7 
14.3 

(Coppet,  A.  ch.  (5)  30.  414.) 
Solubility  is  reoresented  bv  a  straight  line. 

-6 
-5.5 

(Coppet.) 

100  pts.  H2O  dissolve  29.33  pts.  KCl  at  4°, 
45.5  pts.  at  60°.    (Andreae,  J.  pr.  (2)  29.  456.) 

100  pts.  H2O  dissolve  at: 

0°        100°      130°      180° 
29.2      56.5        66         78  pts.  KCl. 
(Tilden  and  Shenstone,  Lond,  R.  Soc.  Proc. 
35.  345.) 

Solubility  of  KCl  in  100  pts.  H2O  at  high 
temp. 


t 

Pts. 
KCl 

t 

Pts. 
KCl 

t° 

Pts. 
KCl 

125 
133 

59.6 
69.3 

147 
175 

70.8 
75.2 

180 

77.5 

(Tilden  and  Shenstone,  Phil.  Trans.  1884.  23.) 


(Meusser,  Z.  anorg.  1905,  44.  80.) 

Sat.  KCl+Aq  at  25°  contains  26.46%  KCl. 
(Foote,  Am.  Ch.  J.  1906,  35.  238.) 

28.01  g.  KCl  are  contained  in  100  g.  solu- 
tion sat.  at  30°.  (de  Waal,  Dissert.  1910.) 

36.12  g.  KCl  are  sol.  in  100  g.  H2O  at  25°. 
(Amadori  and  Pampanini,  Rend.  Ace.  Line. 
1911,  V.  20.  473.) 

4.272  g.  mol.  are  contained  in  1  1.  solution 
sat.  at  25°.  (Herz.  Z.  anorg.  1911,  73.  274.) 

Solubility  of  KBr  at  6°  =  23.06%;  28.4°  = 
26.91%;  62.6°  =  31.57°.  (Sites,  Z.  Krist.  1912, 
61.  262.) 

Solubility  at  22°  =  25.68%.  (Bronstedt,  Z. 
phys.  Ch.  1912,  80.  208.) 

100  mol.  H2O  dissolve  at: 
19.3°        29.7°        40.1°          54.5° 
8.2          8.99          9.75          10.39  mol.  KCl. 
(Sudhaus,  Miner.  Jahrb.  Beil.-Bd.  1914,  37. 
18.) 


750 


POTASSIUM  CHLORIDE 


KCl+Aq  sat.  at   16°  has  sp.  gr.  =  1.077. 
(Stolba,  J.  pr.  97.  503.) 

Sp.  gr.  of  KCl+Aq  at  17.5°. 

A 

Sp.  gr. 

o/ 
KCl 

Sp.  gr. 

KCl 

Sp.  gr. 

i 

2 
3 

4 
5 
6 

7 
.  8 

1.0062 
1.0125 
1.0189 
1.0254 
1.0319 
1.0385 
1.0451 
1.0518 

9 
10 
11 
12 
13 
14 
15 
16 

1.0586 
.0655 
.0725 
.0795 
.0866 
.0937 
.1008 
.1080 

17 

18 
19 
20 
21 
22 
23 
24 

.1152 
.  1225 
.1298 
.1372 
.1446 
.1521 
.1596 
.1673 

(Schiff,  A.  110.  76.) 
Sp.  gr.  of  KCl+Aq  at  19. 

5°. 

%  KCl 

Sp.  gr.              %  KCl 

Sp.  gr. 

5.98 
11.27 
16.27 

1.0382         21.31 
1.0733         25.133 
1  .  1075 

1.1436 
1  .  1720 

(Kremers,  Pogg.  95/119. 
Sp.  gr.  of  KCl+Aq  at  15 

o 

I 

Sp.  gr. 

K%1 

Sp.  gr. 

at 

KCl 

Sp.  gr. 

1 
2 
3 

4 
5 

6 

7 
8 
9 

1.00650 
1.01300 
1.01950 
1.02600 
1.03250 
1.03916 
1.04582 
1.05248 
1.05914 

10 

11 

12 
13 
14 
15 
16 
17 
18 

1.06580 
1.07271 
1.07962 
1.08654 
1.09345 
1  .  10036 
1  .  10750 
1.11465 
1.12179 

19 
20 
21 
22 
23 
24 
24.9* 

1.12894 
1.13608 
,14348 
.  15088 
.  15828 
.  16568 
.17234 

Sp.  gr.  of  KCl+Aq  at  0°.  S=  pts.  salt  in  100 
pts.  of  solution;  Si  =  mols.  salt  in  100 
mols.  solution. 


s 

Si 

Sp.  gr. 

20.7840 
17.7214 
14.4707 
11.0757 
7.5440 
4.4968 

5.954 
4.940 
3.922 
2.918 
1.931 
1.123 

1.1489 
1  .  1258 
1.1018 
1.0769 
1.0521 
1.0308 

(Charpy,  A.  ch.  (6)  29.  23.) 
Sp.  gr.  of  KCl+Aq  at  25°. 


Concentration  of  KCl+Aq 

Sp.  gr. 

1-normal 
Vr-      " 

V4-     " 

Vs-       "     •:••••* 

1.0466 
1  .  0235 
1.0117 
1  .  0059 

(Wagner,  Z.  phys.  Ch.  1890,  5.  36.) 

KCl+Aq  containing  5.05%  KCl  has  sp.  gr. 
20°/20°  =  1.0327. 

KCl+Aq  containing  20.55%  KCl  has  sp. 
gr.  20°/20°  =  1.1393. 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  272.) 

Sp.  gr.  of  KCl+Aq. 


g.  KCl  in  1000  g. 
of  solution 

Sp.  gr.  16°/16° 

0 
0.7140 
1.5042 
3.0724 
8.3165 

1.000000 
1.000464 
1  .  000975 
1.001991  
1.005391 

*  Mother  liquor. 
(Gerlach,  Z.  anal.  8.  281.) 

Sp.  gr.  of  KCl+Aq  at  20°,  containing  mols. 
KCl  to  100  mols.  H2O. 


(Dijken,  Z.  phys.  Ch.  1897,  24.  109.) 

Sp.  gr.  of  KCl+Aq  at  20.1°,  when  p=per 
cent  strength  of  solution;  d=  observed 
density,  and  w=  volume  cone,  in  g.  per 


Mols.  KCl 

Sp.  gr. 

Mols.  KCl 

Sp.  gr. 

0.5 
1.0 
2.0 

1.01310 
1.02568 
1.04959 

4.0 
5.0 

1.09415 
1.11445 

(Nicol,  Phil.  Mag.  (5)  16.  122.) 
Sp.  gr.  of  KCl+Aq  at  18°. 


A 

IvUl 

Sp.  gr. 

A 

.Kd 

Spigr. 

% 

JvUl 

Sp.  gr. 

5 

10 

1.0308 
1.0638 

15 
20 

1.0978 
1.1335 

25 

1.1408 

(Kohlrausch,  W.  Ann.  1879.  1.) 


cc-  (m)=w 

p 

d 

w 

36.43 

1.853 

0.43171 

31.12 

.1554 

0.35954 

24.79 

.1215 

0.27887 

18.06 

.0866 

0.19610 

13.17 

,QB1Z  

8.412 

.0386 

~~  o!  08736 

6.610 

.0297 

0.06806 

4.419 

1.0193 

0.4505 

3.456 

1.0148 

0.03507 

1.197 

1.0040 

0.01202 

.   (Barnes,  J.  phys.  Ch.  1898,  2.  544.) 

POTASSIUM  CHLORIDE 


751 


Sp.  gr.  of  KCl+Aq  at  t°. 

KCl+Aq    containing    10%   KCl   boils   at 
101.1°;  containing  20%,  at  103.4°.    (Gerlach.) 
Sat.  KCl+Aq  containing  52.7  pts.  KCl  to 
100  pts.  H2O  forms  a  crust  at  107.7°;  highest 
temp,  observed,  108.5°.    (Gerlach,  Z.  anal.  26. 
426.) 

B.-pt.  of  KCl+Aq  containing  pts.  KCl  to 
100  pts.  H2O.    G=  according  to  Gerlach 
(Z.    anal.    26.    438);    L=  according    to 
Legrand  (A.  ch.  (2)  59.  426). 

t° 

Normality  of 
KCl+Aq. 

g.  KCl  in 
100  g.  of 
solution 

Sp.  gr.  t°/4° 

20.5 

it 

it 

<( 

3.74 
2.65 

1.87 
0.93 

23.93 
17.66 
12.82 
6.64 

1.1617 
1.1166 
1.0829 
1.0424 

(Oppenheimer,  Z.  phys.  Ch.  1898,  27.  450.) 
Sp.  gr.  of  KCl+Aq  at  18°/4°. 

B.-pt. 

G 

L 

B.-pt. 

G 

L 

100.5° 
101.0 
101.5 
102 
102.5 
103 
103.5 
104 
104.5 

4.9 
9.2 
13.1 
16.7 
20.1 
23.4 
26.7 
29.9 
33.1 

4.7 
9.0 
13.2 
17.1 
20.9 
24.5 
28.0 
31.4 
34.6 

105° 
105.5 
106 
106.5 
107 
107.5 
108 
108.3 
108.5 

36.2 
39.3 
42.4 
45.5 
48.4 
51.5 
54.5 

57.'4 

37.8 
41.0 
44.2 
47.4 
50.5 
53.7 
56.9 
59.4 

g.  KCl  in  100  g. 
of  solution 

Sp. 

gr. 

0.24963 
0.12459 
0.08342 
0.062343 

1.0003 
0.9995 
0.99929 
0.99912 

(Jahn,  Z.  phys.  Ch.  1900,  33.  559.) 

KCl+Aq  containing  1  pt.  KCl  in  58.923 
pts.  H2O  at  17°  has  sp.  gr.  =  ]  .0096.  (Hittorf, 
Z.  phys.  Ch.  1902,  39.  628.) 

Sp.  gr.  20°/4°  of  a  normal  solution  of  KCl  = 
1.04443.  (Haigh,  J.  Am.  Chem.  Soc.  1912, 
34.  1151.) 


Precipitated  from  aqueous  solution  by  HC1 
+Aq.  Much  less  sol.  in  very  dil.  HCl+Aq 
than  in  H2O.  (Fresenius.) 

Nearly  insol.  in  cone.  HCl+Aq. 

100  cc.  sat.  HCl+Aq  dissolve  1.9  g.  KCl 
at  17°.  (Ditte,  A.  ch.  1881,  (5)  24.  226.) 


—     Sp.  gr.  of  sat.  KCl+Aq  at  t°. 

G.  per  100  cc.  of  solution 

t° 

g.  KCl 
100  g. 

sol.  in 
H20 

Sp.  gr. 

HC1 

KCl 

—10° 
0 
10 
20 
30 
40 
50 
60 
70 

24.98 
28.50 
31.23 
34.11 
37.28 
40.12 
42.86 
45.48 
48.30 

1.139 
1.156 
1.168 
1.177 
1.183 
1.190 
1.195 
1.199 
1.203 

0.0 
1.42 
2.41 
2.59 
4.05 
8.39 
12.40 
14.95 
23.88 
54.20 

25.73 
22.69 
20.84 
20.51 
17.71 
11.93 
7.46 
5.60 
1.49 
1.52 

(Tschernaj,  J.  Russ.  phys.  Chem.  Soc.  1912, 
44.  1565.) 

Sp.  gr.  of  dil.  KCl+Aq  at  20.004°. 
Conc.=  g.  equiv.  KCl  per  1.  at  20.004°. 
Sp.  gr.  compared  with  H2O  at  20.  004°=  1. 

(Engel,  A.  ch.  1888,  (6)  33.  377.) 
Solubility  of  KCl  in  HCl+Aq. 

t° 

Concentra- 
tion of  HC1 
g.  mol.  per 
1000  g.  H2O 

Wt.  KCl  per 
1000  g.  H20 

Mol. 
solubility 

Cone. 

Sp.  gr. 

0 

u 

ft 
ti 

Q 

\ 

283.55 
267.25 
250.00 
214.25 

3,81 
3.59 
3.36 

2.88 

0.0000 
0.0001 
0.0002 
0.0005 
-0.0010 
0.0026 
0.0050 
0.0100 

1.000,000,0 
1.000,004,8 
1.000,009,7 
1.000,024,2 
1.000,048,5 
1.000,097,1 
1.000,242,6 
1.000,483,6 

25 
n 

ti 
it 

0 

1A 
Y* 
l 

359.25 
341.55 
324.30 
289.60 

4.82 
4.59 
4.35 
3.89 

(Lamb  and  Lee,  J.  Am.  Chem.  Soc.,  1913,  36. 
1687.) 

(Armstrong  and  Eyre,  Proc.  R.  Soc.  1910  (A) 
84.  127.) 

752 


POTASSIUM  CHLORIDE 


100  g.  sat.  HCl+Aq  dissolve  1.9  g.  KG 
at  20°.    (Stoltzenberg,  B.  1912,  46.  2248.) 


Solubility  in  HCl+Aq  at  25°. 


Millimols  HC1  in  10  ccm.     Millimols  KC1  in  10  ccm. 


5.66 
10.20 
15.90 
20.94 
32.52 


42.72 
37.49 
33.79 

28.68 
24.74 
17.39 


Solubility  of  KC1  in  MgCl2+Aq  of  given  per- 
centage composition. 


10 
20 
30 
40 
50 
60 
70 
80 
90 
100 


30% 


1.9% 

2.6 

3.4 

4.2 

5.0 

5.8 

6.5 

7.3 

8.1 

8.9 


21.2% 


5.3% 

6.5 

7.6 

8.8 
10.0 
11.2 
12.4 
13.6 
14.7 
15.9 


15% 


9.9% 
11.3 
12.7 
14.2 
15.6 
17.0 
18.3 
19.5 
20.8 
22.1 


14.3% 

15.9 

17.5 

19.0 

20.5 

21.9 

23.2 

24.5 

25.8 

27.1 


(Herz,  Z.  anorg.  1912,  73.  275.) 


Solubility  of  KC1  in  HBr+Aq  at  25°. 


Millimols  HBr  in  10  ccm.     Millimols  KC1  in  10  ccm 


6.61 

34.15 


42.72 
37.80 
19.57 


(Herz,  Z.  anorg.  1912,  73.  275.) 


Sol.  in  sat.  NH4Cl+Aq  with  pptn.  of 
NH4C1.  When  action  has  ceased,  the  solu- 
tion at  18.75°  contains  31.6%  of  the  mixed 
salt:  or  100  pts.  H2O  dissolve  46.1  pts.  of  the 
mixed  salt,  viz,  16.27  pts.  KC1  and  29.83 
pts.  NH4C1.  (Karsten.) 


Solubility  of  KC1  in  NH4Cl+Aq  at  25°. 


Dissolved  in  1000  mols  H2O. 


Mols  KC1 

Mols  NH4C1 

74.2 

23.8 

67.9 

32.5 

61.4 

52.2 

55.5 

65.9 

50.2 

74.4 

43.0 

96.3 

37.6 

110.0 

37.0 

107.5 

37.5 

109.4 

22.6 

118.2 

(Biltz,  Z.  anorg.  1911,  71.  174.) 
See  also  NH4C1. 

Sol.  in  sat.  BaCl2+Aq  with  pptn.  of  BaCl2 
until  a  state  of  equilibrium  is  reached,  when 
100  pts.  H2O  at  16.8°  dissolve  45.9  pts.  mixed 
salts,  viz.  18.2  pts.  BaCl2  and  27.7  pts.  KCl. 

See  also  BaCl2. 


(Precht  and  Wittgen,  B.  14.  1667.) 
Solubility  of  KCl+NaCl  in  20%  MgCl2+Aq. 


10 
20 
30 
40 
50 


%KC1 


4.2 
5.1 
6.0 
6.9 
7.9 


5.7 

5.8 
5.9 
6.0 
6.1 


60 
70 
80 
90 
100 


%  KCl 


8.9 

9.9 

10.9 

11.9 

13.0 


6.3 
6.4 
6.6 
6.7 
6.9 


(P.  and  W.) 
Sol.  in  sat.  KNO3+Aq  with  pptn.  of  KNO3. 


1  litre  of  the  solution  contains 


at  14.5C 


Mol.  KC1      Mol.  KNOj 


3.865 
3.S10 
3.782 
3.710 
3.667 
3.629 
3.597 
3.582 


0.0 

0.204 

0.318 

0.615 

0.818 

0.910 

1.176 

1.220 


at  25.2° 


Mol.  KC1       Mol.  KN08 


18 
11 
07 
93 

85 
81 


3.70 


0.0 

0.136 

0.318 

0.902 

1.212 

1.397 

1.805 


(Touren,  C.  R.  1900,  130.  909.) 
Solubility  of  KC1  in  KNO3+Aq. 


25 


Concentra- 
tion of  KNO3 
in  g.  mol. 
per  1000  g. 
H20 


0 


o 

I 


Wt.  KCl  in 
1000  g.  H2O 


283.55 
284.25 
283.60 
287.60 
364.15 
355.00 
361.65 
358.80 
355.20 


Mol. 
solubility 


3.81 
3.81 
3.81 
3.86 
4.89 
4.90 
4.86 
4.81 
4.77 


Armstrong  and  Eyre,  Proc.  R.  Soc.  1910  [A], 

84.  127.) 
See  also  KNO3. 


POTASSIUM  CHLORIDE 


753 


Sol.  in  sat.  NaNO3-f  Aq  without  causing 
pptn.    (See  NaNO3.) 
Sol.  in  sat.  Ba(NO3)2+Aq  without  causing 
pptn. 
Solubility  in  KBr+Aq  at  25.2°. 

Solubility  of  KC1  in  KOH+Aq  at  0°. 

G.  per  100  cc.  solution 

KC1 

KOH 

1  litre  of  the  solution  contains 

26.83 
23.44 
21.39 
17.39 
13.89 
10.91 
8.64 
6.78 
4.74 

0.0 
1.33 
2.64 
5.56 
8.46 
11.23 
13.83 
16.43 
19.72 

Mol.  KBr 

Mol.  KC1 

0.0 
0.49 
0.85 
1.31 
1.78 
2.25 
2.69 

4.18 
3.85 
3.58 
3.19 
2.91 
2.58 
2.33 

(Engel,  Bull.  Soc.  1891,  (3)  6.  16.) 

(Touren,  C.  R.  1900,  130.  1252.) 
See  also  KBr. 

100  pts.  H2O  dissolve  133.2  pts.  KI  and 
10.4  pts.  KC1  at  21.5°,  no  matter  how  pre- 
pared. (Rtidorff,  B.  6.  484.) 

100  pts.  KCl+Aq  sat.  at  15-16°  contain 
25.26-25.37  pts.  KC1.  100  pts.  KCl+Ki  + 
Aq  sat.  at  15-16°  contain  57.80  pts.  of  the  two 
salts.  KC1  is  pptd.  by  KI.  (v.  Hauer.  J.  pr. 
98.  137.) 

Solubility  in  KI+Aq  at  t°. 


t° 

Sat.  solution  contains 

%KC1 

%  KI 

%  total  salt 

0 

4.8 

50.8 

56.6 

8 

5.1 

51.1 

56.2 

18 

57.9 

30 

4^2 

54^6 

58.8 

41 

4.7 

55.0 

59.7 

49 

5.7 

56.0 

61.7 

60 

62.5 

75 

4.4 

59^5 

63.9 

82 

5.0 

59.6 

64.6 

96 

. 

66.2 

102 

.  .  . 

66.8 

140 

• 

63^3 

155 

'7.'6 

64.8 

7214 

182 

8.7 

65.4 

74.1 

190 

8.6 

66.0 

74.6 

245 

10.0 

66.5 

76.$ 

(fitard,  A.  ch.  1894,  (7)  3.  281.) 
Solubility  of  KCl+KI  in  H20  at  25°. 


G.  per  100  g.  H2O 


KC1 

KI 

KCl 

KI 

0 
4.06 
7.63 
11.36 
11.74 
15.10 

149.26 
144.03 
137.79 
132.60 
133.90 
105.91 

19.64 
23.75 
29.56 
31.38 
33.68 
36.12 

68.22 
43.89 
23.83 
14.83 
7.00 
0.00 

(Amadori  and  Pampanini,  Att.  Ace.  Line. 
1911,  20,  II.  475.) 


Solubility  in  KOH+Aq  at  20°, 


G.  KOH  in 
1  litre 

G.  KC1  in 
1  litre 

Sp.  gr. 

Degrees 
Baum6 

10 

293 

.185 

22.5 

20 

285 

.185 

22.5 

30 

276 

.190 

23.0 

40 

265 

.192 

23.0 

50 

255 

.195 

23.5 

60 

245 

.200 

24.0 

70 

236 

.200 

24.0 

80 

226 

.205 

24.5 

90 

219 

1.205 

24.5 

100 

211 

1.210 

25.0 

110 

205 

1.210 

25.0 

120 

199 

1.215 

25.5 

130 

192 

1.215 

25.5 

140 

185 

1.220 

26.0 

150 

178 

1.225 

26.5 

160 

171 

1.225 

26.5 

170 

165 

1.230 

27.0 

180 

159 

1.235 

27.5 

190 

153 

1.240 

28.0 

200 

148 

1.245 

28.5 

210 

142 

1.250 

29.0 

220 

137 

1.255 

29.5 

230 

133 

1.260 

30.0 

240 

128 

1.265 

30.5 

250 

124 

1.270 

30.8 

260 

120 

1.275 

31.3 

270 

115 

1.280 

31.7 

280 

112 

1.285 

32.0 

290 

108 

1.290 

32.5 

300 

104 

1.295 

33.0 

310 

ioo 

1.300 

33.5 

320 

96 

1.305 

34.0 

330 

93 

1.310 

34.2 

340 

89 

1.315 

34.6 

350 

85 

1.320 

35.0 

360 

81 

1.325 

35.5 

370 

78 

1.330 

36.0 

380 

74 

1.335 

36.3 

390 

71 

1.340 

36.7 

400 

68 

1.345 

37.1 

410 

64 

1.350 

37.5 

754 


POTASSIUM  CHLORIDE 


Solubility  in  KOH+Aq  at  20°.—  -Continued. 

Solubility  of  KCl+NaCl  in  H2O  at  t°.    100 
pts.  H2O  dissolve  pts.  KCl  and  pts.  NaCl. 

G.  KOH  in 
1  litre 

G.  KCl  in 
1  litre 

Sp.  gr. 

Degrees 
Baum6 

Pts. 
KCl 

Pts. 
NaCl 

Pts. 
KCl 

Pts. 

NaCl 

420 
430 
440 
450 
460 
470 

61 
58 
55 
53 
50 
47 

:355 
.360 
.365 
.370 
.375 
.380 

38.0 
38.5 
38.9 
39.2 
39.5 
40.0 

TO       12.5 
20       14.7 
30       17.2 
40        19.5 
50       22.0 

29.7 
29.2 

28.7 
28.2 
27.7 

60        24.6 
70       27.3 
80        30.0 
90       32.9 
100        34.7 

27.2 

26.8 
26.4 
26.1 

25.8 

480 
490 

44 
42 

.385 
.390 

40.2 
40.6 

(Precht  and  Wittgen,  B.  14.  1667.) 

500 
510 
520 
530 

40 
38 
35 
33 

.397 
.405 
.410 
.415 

41.0 
41.5 
42.0 
42.3 

100  pts.  H2O  dissolve  13.99  pts.  KC1+30.54 
pts.     NaCl  =  44.53  pts.  mixed  salts  at  20°. 
(Nicol,  Phil.  Mag.  (5)  31.  385.) 

540 

31 

.420 

42.6 

550 

KftfV 

29 

97 

.425 

1    4.^0 

43.0 

/iq    K 

Solubility  of  KCl  in  NaCl+Aq  at 

20°. 

570 

25 

1.435 

43.7 

G.  per  100  g.  H2O 

580 

24 

1.440 

44.0 

NaCl 

KCl 

590 

23 

1  445 

44  3 

600 

22 

1.450 

44.6 

0.0 

34.52 

610 

21 

1.455 

45.0 

6.5 

29.37 

620 

20 

1.460 

45.5 

13.0 

4.71 

630 

18 

1.465 

45.9 

19.5 

0.42 

640 

17 

470 

46  2 

650 

16 

.475 

46.5 

(Nicol,  Phil.  Mag.  1891,  31.  369 

.) 

660 

15 

.480 

46.8 

670 

680 

15 
15 

.485 
.490 

47.0 
47.5 

Solubility  of  KCl+NaCl  at  t°. 

690 

15 

.495 

47.9 

G.  per  100  g.  H2O 

7OO 

14. 

KAA 

AQ     9 

710 

14 

.505 

48.5 

KCl                           NaCl 

720 
730 

13 
13 

.510 
.515 

48.8 
49.1 

25 

15.8                    14 

.5 

740 

13 

.520 

49.5 

1C 

29.0                   31 

.3 

750 

13 

.525 

49.7 

80 

30.0                   25 

.2 

760 

12 

.530 

50.0 

n 

26.4                    34 

.0 

770 

780 

12 
12 

.535 
.540 

50.3 
50.6 

(Soch,  J.  phys.  Ch.  1898,  2.  46. 

) 

790 

11 

.545 

51  0 

800 

11 

.550 

51.3 

Solubility  of  KCl+NaCl  at  ?  ° 

810 

820 

10 
10 

.560 
.565 

51.5 
51.8 

G.  salts  in  100  g.  H2O 

830 

9 

1.570 

52.2 

NaCl 

KCl                      Solid  phase 

840 

1    £.7^ 

co    a 

850 

9 

1.580 

53.0 

9.89 

28.34                  KCl 

1  R    ^P» 

22  75                      " 

(Winteler,  Z.  Elektrochem,  1900,  7.  360.) 

29.88 
31.57 

16.28             KCl+NaCl 
10.91                  NaCl 

33.17 

5.65 

KCl+NaCl. 

100  pts.  KCl+NaCl+Aq  sat.  at  13-16° 
contain  30.18  pts.  of  the  two  salts,  (v. 
Hauer.) 

100  pts.  H2O  dissolve  13.92  pts.  KCl  and 
30.65  pts.  NaCl  at  15.6°,  and  solution  has 
sp.  gr.  =  1.233.  (Page  and  Keightley.) 

100  pts.  H2O  dissolve  10.11  pts.  KCl,  32.15 

Ets.  NaCl,  and  4.69  pts.  K2SO4,  and  solution 
as  sp.  gr.  =  1.250.    (P.  and  K.) 

100  pts.  H2O  dissolve  29.9  pts.  NaCl  and 
15,7  -pts.-KCl  at  18.8°.  (Riidorff.)- 


(Uyeda,  Mem.  Col.  Sc.  Kioto,  1910,  2.  245.) 

100  g,  H2O  sat.  .with  NaCl  dissolve  0.216 
gram-equivalent  KCl  at  25°. 
*  100  g  H2O  sat.  with  K2SO4  dissolve  0.466 
gram-equivalent    KCl    at    25°.      (Euler,    Z. 
phys.  Ch.  1904,  49.  315.) 

Solubility  in  NaCl+Aq  at  20°,  30°,  40°  and 
91°.  Tables  given  in  the  original  show  that 
each  salt  diminishes  the  solubility  of  the 
other.  (Leather,  Chem.  Soc.  1915,  108.  (2) 
13.) 


POTASSIUM  CHLORIDE 


755 


Solubility  of  KCl+NaCl  in  HCl+Aq  at  25°. 


%HC1 

%NaCl 

%KC1 

0 
8.61 
17.16 
20.65 
32.78 

19.95 
10.65 
3.56 
2.03 
0.18 

10.90 
7.58 
3.80 
2.86 
1.27 

(Hicks,  J.  Am.  Chem.  Soc.  1915,  37.  846.) 
See  also  under  NaCl. 

KCl+SrCl2. 

100  pts.  H2O  dissolve  11.2  pts.  KC1  and 
48.6  pts.  SrCl2  at  14.5°.    (v.  Hauer.) 

If  SrCl2+Aq.  sat.  at  14.5  is  sat.  with  KC1 
at  same  temp.,  100  pts.  H2O  dissolve: 


KC1      .      .      . 
SrCl2    .      .     . 

33.2 

11.2 
48.6 

50!7 

59.8 

(Mulder,  Scheik.  Verhandel.  1864.) 

KC1+(NH4)2SO4. 

Sat.  solution  of  KC1  +  (NH4)2SO4  at  b.-pt. 
when  cooled  to  14°  has  different  composition 
from  sat.  solution  of  (NH4)C1  and  K2SO4,  and 
its  composition  is  changed  by  warming  it  with 
either  KC1  or  (NH4)2SO4.  (Riidorff.) 

KC1+K2SO4. 

100  pts.  H2O  contain  the  following  amounts 
salt  at  18.75°:  (1)  sat.  with  KC1  alone; 

(2)  sat.  first  with  KC1  then  with  K2SO,; 

(3)  sat.  with  K2SO4  and  KC1  together; 

(4)  sat.  first  with  K2SO4  then  with  KC1; 

(5)  sat.  with  K2SO4  alone. 


KC1       . 

K2S04   . 

i 

2 

3 

4 

5 

34.5 

32.96 
1.79 

33.12 
1.75 

33.12 
1.83 

iols 

(Karsten.) 

100  pts.  H2O  sat.  with  both  K2S04  and  KC1 
contain  the  following  amounts. 


KC1 
K2S04  .     .     . 

At  14.8° 

33.5 

28.2. 
2.0 

1613 

KC1 

K2S04  .     .     . 

At  15.8° 

33.6 

27.9 
2.3 

16!4 

KC1 

K2S04  .     .     . 

At  16.1° 

33.6 

27.1 
3.3 

16!  4 

(Kopp,  A.  34.  264.) 


Sat.  K2SO4+Aq  dissolves  KC1  only  with 
pptn.  of  K2SO4,  but  sat.  KCl+Aq  dissolves 
some  K2SO4  without  any  separation.  (Kar- 
sten.) 

Solubility  of  KC1+K2SO4:     100  pts.   H2O 
dissolve  at  t°. 


t° 

Pts. 
KC1 

Pts. 
K2S04 

t° 

Pts. 
KC1 

Pts. 
K2S04 

10 
20 
30 
40 
50 

30.9 
33.4 
36.1 
38.7 
41.3 

1.32 
1.43 
1.57 
1.68 
1.82 

60 
70 
80 
90 
100 

43.8 
46.5 
49.2 
52.0 
54.5 

1.94 
2.06 
2.21 

2.38 
2.53 

(Precht  and  Wittgen.) 

100  g.  H2O  dissolve  34.76  g.  KC1+2.93  g. 
K2SO4  at  25°.  (Van't  Hoff  and  Meyerhoffer, 
Z.  phys.  Ch.  1898,  27.  75.) 

Sol.  in  20%  KC2H3O2+Aq.    (Stromeyer.) 

Quickly  attacked  by  liquid  NO2  in  the 
presence  of  traces  of  moisture,  with  evolution 
of  C12.  (Frankland,  Chem.  Soc.  1901,  79. 
1361.) 

SI.  sol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Easily  sol.  in  liquid  HF.  (Franklin,  Z. 
anorg.  1905,  46.  2.) 

100  g.  hydrazine  dissolves  8.5  pts.  KC1  at 
12.5-13°.  (de  Bruyn,  R.  t.  c.  1899,  18.  297.) 

100  g.  anhyd.  hydroxylamine  dissolve  12.3 
g.  KC1  at  17-18°.  (de  Bruyn,  Z.  phys.  Ch. 
1892,  10.  782.) 

100  pts.  alcohol  of  0.900  sp.  gr.  dissolve  4.62  pts.; 

0.872,  1.66  pts.;  0.834,    0.38  pt.;  0.817,  0.00  pt.  KC1. 

(Kirwan.) 

Sol.  in  48  pts.  boliing  alcohol.     (Wenzel.) 
Insol.  in  absolute  alcohol  containing  LiCl.     (Mits- 

cherlich.) 


15°,  100  pts.  alcohol  of  p  percenta 
ae   (S  =  sp.    gr.)    dissolve  pts.   K< 


At 

volume 
follows: 

10 

0.984 
KC1       19.8 


20 

0.972 
14.7 


30 

0.958 
10.7 


KC1 


50 

0.918 
5.0 


60 
0.896 

2.8 


;e  by 
1   as 

40 
0.940 

7.7 

80 

0.848 
0.45 


(Schiff,  A.  118.  365.) 


100  pts.  of  a  mixture  of  40%  alcohol  with 
60%  H2O  dissolve  9.2' pts.  KC1  at  15°. 
(Schiff.) 

Insol.  in  absolute  alcohol  or  in  96%  alcohol 
at  15°  or  below.  At  20°,  100  pts.  of  the  latter 
dissolve  0.04  pt.;  at  25°,  0.06  pt.;  at  30°,  0.20 
pt.  KC1.  Dilute  alcohol  dissolves  less  KC1 
than  the  contained  H2O  would  dissolve  by 
itself. 


756 


POTASSIUM  CHLORIDE 


Solubility  in  dil.  alcohol.    D  =  sp.  gr.  of  alco- 
hol; S  =  solubility  in  100  pts.  alcohol  at  t°. 

Solubility  of 

KCl  in  ethyl  alcohol  at  0°. 

Concentration  of 
alcohol     Mol.  g. 
alcohol  per  1000 
g.H20 

Solubility  in 
1000  g.  H20 

Molecular 
solubility 

D  =0.9904 

D  =0.9848 

D  =0.9793 

D  =0.9726 

t° 

S 

t° 

s 

t 

S 

t° 

s 

0^25 
0.50 

1.00 
3.00 

285.15 
277.95 
271.10 
265.50 

208.80 

3.80 

3.73 
3.64 
3.45 

2.81 

0 
4 
22 
25 
34 
52 

23.2 

24.8 
29.4 
30.2 
32.8 
37.5 

4 
20 
27 
30 
37 
60 

20.9 
25.5 
26.6 
27.5 
29.0 
35.2 

4 
21 
28 
43 

16.4 
20.3 
22.0 
25.6 

3 
5 
16 
20 
25 
34 

12.2 
12.7 
15.4 
16.1 
17.3 
19.0 

(Armstrong  and  Eyre,  Proc.  Rov.  Soc.  1910. 
(A)  84.  127.) 

Solubility  of  KCl  in  ethyl  alcohol  +Aq  at 
25°. 

D  =0.9573 

D  =0.9390 

D  =0.8967 

D  =0.8244 

t° 

S 

t/ 

s 

t 

s 

t 

S 

10 

11 

17 
30 
40 
60 

8.8 
9.0 
10.3 
12.5 
13.9 
16.7 

2 

7 
16 
30 
38 
57 

4.2 
5.1 
6.4 
8.5 
9.6 
11.3 

12 
31 

47 
65 

2.87 
4.35 
4.88 
5.65 

4 
15 
20 
25 
32 

0.00 
0.00 
0.04 
0.06 
0.20 

wt.  % 

alcohol 

G.  KCl  per 
100  cc. 
sat.  solution 

wt.  %  ' 

alcohol 

G.  KCl  per 
100  cc. 
sat.  solution 

(Gerardin,  A.  ch.  (4)  6.  140.) 
Solubility  of  KC1  in  dil.'  alcohol  at  14.5° 

0 
10 
20 
30 
40 
50 

31.18 
23.93 
17.89 
13.27 
9.40 
6.26 

60 
70 
80 
90 
100 

4.18 
2.27 
0.93 
0.31 
0.08 

Sp.  gr. 

100  ccm.  contain 

CMcIntosh,  J.  phys.  Ch.  1903,  7.  350.) 

100  pts.  absolute  methyl  alcohol  dissolve 
0.5  pt.  at  18.5°;  100  pts.  absolute  ethyl  al- 
cohol dissolve  0.034  pt.  at  18.5°.    (de  Bruyn, 
Z.  phys.  Ch.  10.  783.) 
100  pts.  40%  wood  alcohol  dissolve  9.2  pts. 
KCl.    (Schiff.) 

Solubility  of  KCl  in  methyl  alcohol+Aq  at 
25°. 

Alcohol 

Water 

KCl 

1.1720 
1.1542 
1.1365 
1.1075 
1.1085 
1.0545 
1.0455 
0.9695 
0.9315 
0.8448 

2^79 
4.98 
10.56 
15.57 
20.66 
24.25 
40.42 
48.73 
68.63 

88.10 
85.78 
84.00 
79.63 
75.24 
70.52 
67.05 
50.18 
40.60 
15.55 

29.10 
26.85 
24.67 
20.56 
17.24 
14.27 
13.25 
6.35 
3.82 
0.30 

(Bodlander,  Z.  phys.  Ch.  7.  316.) 

Solubility  of  KCl  in  ethyl  alcohol. 
(G.  KCl  per  100  g.  alcohol+Aq.) 


P  =  %  by  wt.  of  alcohol  in  alcohol+Aq. 
S  =Sp.  gr.  alcohol+Aq  sat.  with  KCl. 
L  =  millimols  KCl  in  100  ccm.  of  the  solu- 
tion. 


wt.  % 

alcohol 

at  30° 

at  40° 

wt.  % 

alcohol 

at  30° 

at  40° 

0 

38.9 

41.8 

43.1 

11.1 

13.1 

5.28 

33.9 

35.9 

55.9 

6.8 

8.2 

9.43 

30.2 

33.3 

65.9 

3.6 

4.1 

16.9 

24.9 

27.6 

78.1 

1.3 

1.6 

25.1 

19.2 

21.8 

86.2 

0.4 

0.5 

34.1 

15.6 

17.2 

(Bathrick,  J.  phys.  Ch.  1896,  1.  160.) 


p 

S  25°/4° 

L 

0 
10.6 
30.8 
47.1 
64.0 
78.1 
98.9 
100 

1.1782 
1.125 
1.033 
0.9679 
0.9064 
0.8607 
0.8242 
0.7937 

417.4 
329 
183 
102 
46.1 
20.6 
9.9 
5.7 

(Herz  and  Anders,  Z.  anorg.  1907,  56.  273.) 

POTASSIUM  CHLORIDE 


757 


Solubility  of  KC1  in  methyl  alcohol. 

500  mg.  KC1  treated  with  10  g.  of  above 

Concentra- 

mixture yield   only  0.3   mg.    to   the  liquid. 
(Lawren.ce  Smith,  Am.  J.  Sci.  16.  56.) 

t° 

tion  of 
alcohol. 
Mol.  g. 

Solubility 
1  in  1000  g. 
wo 

Molecular 
solubility 

Insol.  in  acetone.     (Krug  and  M'Elroy,  J. 
Anal.  Ch.  6.  184;  Eidmann,  C.  C.  1899,  II. 

alcohol  per 
1000  g.  H2O 

JX2Vj 

1014.) 

0 
ii 

6!25 

283.55 
280.00 

3.81 
3.76 

Solubility  of  KC1  in  acetone+Aq  at  t.° 

ii 

0.50 

276.35 

3.71 

100  g.  of  the  solution  contain 

ii 

1.00 

267.85 

3.60 

% 

a 

3.00 

238.10 

3.18 

t 

acetone 

G.  H2O 

G.  acetone 

G.KCl 

25 

364.15 

4.89 

30 

0 

72.73 

0.00 

27.27 

a 

•  0.25 

361.90 

4.86 

5 

71.15 

3.74 

25.11 

SI 

0.50 

357.10 

4.79 

9.09 

69.62 

6.96 

23.42 

11 

1.00 

348.70 

4.67 

20 

64.88 

16.22 

18.90 

II 

3.00 

324.15 

4.35 

30 

59.49 

25.45 

15.06 

4-O 

rQ    17 

QK     CO 

Uqi 

(Armstrong  and  Eyre,  Proc.  Roy.  Soc.  1910 
(A)  84.  127.) 

TtU 

50 
60 

OO  .  -L  * 

45.98 
37.97 

OO  .  O^ 

45.98 
56.91 

.  OJ- 

8.04 
5.12 

70 

29.22 

68.18 

2.60 

At  room  temp.  1  pt.  by  weight  is  sol.  in: 
200  pts.  methyl  alcohol,  D15  0.7990. 
750    "    ethyl          "        D15  0.8035. 

80 
90 
100 

19.82 
9.98 
0.00 

79.43 
89.88 
100.00 

0.76 
0.13 
0.00 

Insol.    in   propyl   alcohol.      (Rohland,    Z. 
anorg.  1899,  18.  325.) 
100  g.  methyl  alcohol  dissolve  0.53  g.  KC1 
at  25°. 

40 

0 
5 

9.09 

71.31 
69.62 

67.88 

0.00 
3.67 
6.79 

28.69 
26.72 
25.33 

100  g.  ethyl  alcohol  dissolve  0.022  g.  KC1 
at  25°. 

15 
20 

65.15 
62.97 

11.51 
15.75 

32.34 
21.28 

100  g.  propvl  alcohol  dissolve  0.004  g.  KC1 
at  25°. 

80 

85 

19.81 
14.94 

79.34 
84.66 

0.58 
0.40 

100  g.  isoamyl  alcohol  dissolve  0.0008  g. 
KC1  at  25°. 

90 
95 

10.00 
4.97 

89.84 
94.96 

0.16 
0.07 

(Turner  and  Bissett,  Chem.  Soo.  1913,  103. 

100 

0.00 

100.00 

0.00 

1909.) 

Sinnck    +Viof£*    ia     Vin-f     f\r\c*    li^nirl     YtV*aoa    V»*vt*/\ 

Insol.   in   propyl   alcohol.      (Schlamp,    Z. 
phys.  Ch.  1894,  14.  276.) 

Solubility  of  KC1  in  propyl  alcohol. 


t° 

Concentra- 
tion of 
alcohol. 
Mol.  g.  per 
1000  g.  H2O 

Solubility  in 
1000  g.  H20 

Molecular 
solubility 

0 

(1 

0^25 

0.50 
1.00 

283.55 
274.10 
265.45 
248.0 

3.81 
3.68 
3.56 
3.33 

25 

it 

u 
it 

0^25 
0.50 
1.00 

365.10 
355.40 
347.70 
331.50 

4.90 

4.77 
4.67 
4.45 

(Armstrong  and  Eyre,  Proc.  Roy.  Soc.  1910, 
(A)  84.  127.) 

Insol.  in  fusel-oil.  (Gooch,  Am.  Ch.  J.  9. 
53.) 

Very  si.  sol.  in  mixture  of  equal  pts.  ab- 
solute alcohol  and  ether.  (Berzelius.) 


these  figures  represent  the  solubility  of  KC1  in 
acetone+Aq  at  30°  and  40°. 

(Snell,  J.  phys.  Chem.  1898,  2.  484.) 

The  addition  of  KC1  to  mixtures  of  acetone 
and  H2O  will  cause  a  division  into 
two  layers.  The  following  table  gives 
the  temp,  at  which  sat.  solutions  of  KC1 
in  acetone+Aq  of  varying  concentra- 
tions separate  into  two  layers  and  also 
the  compositions  of  the  sat.  solutions  of 
KC1  in  acetone+Aq. 


% 

acetone 

Temp, 
of 
division 

100  g.  of  solution  contain 

G.H20 

G.  acetone 

G.KCl 

26 

46.5° 

30 

40.0 

59.36 

25.44 

15.20 

40 

34.2 

53.21 

35.47 

11.32 

50 

32.6 

45.97 

45.97 

8.06 

60 

33.3 

37.86 

56.80 

5.34 

70 

35.5 

29.09 

68.25 

2.66 

75 

39.0 

80 

45.6 

19.80 

79.20 

1.00 

(Snell.) 


758 


POTASSIUM  CHLORIDE 


The  following  table  gives  the  compositions  of 
the  solutions  of  KCl  in  acetone +Aq  at 
the  points  at  which  the  solution  just 
divides  into  two  layers.  Temp.  =  40°. 

100  g.  of  the  solution  contain 


Solubility  in  acetone +Aq  at  20°. 
A=ccm.  acetone  in  100  ccm.  acetone+Aq. 
KCl=millimols  KC1  in  100  cem.  of  the 
solution. 


G.  H20 

G.  acetone 

G.  KCl 

56.68 

28.63 

14.68 

53.05 

35.67 

11.29 

50.34 

39.82 

9.83 

47.60 

43.83 

8.58 

44.35 

48.36 

7.29 

42.68 

50.75 

6.57 

38.53 

56.26 

5.21 

36.59 

58.84 

4.57 

32.37 

64.18 

3.45 

30.62 

66.43 

2.95 

28.12 

69.45 

2.44 

A 

KCl 

0 

410.5 

10 

351.7 

20 

286.6 

30 

223.7 

40 

166.5 

50 

115.4 

60 

71.2 

.  $    70 

38.5 

80 

12.9 

90 

2.0 

100 

(Herz  and  Knoch,  Z.  anorg.  1904,  41.  317.) 

(Snell.) 


Solubility  of  KCl  in  glycerine +Aq  at  25°. 
G=g.  glycerine  in  100  g.  glycerine+Aq. 


The   addition   of  KCl  to   aqueous   acetone 
causes  the  separation  of  the  liquid  into 
two  layers.    The  following  table  gives  the 
composition  of  these  layers  at  40°. 

KCl  =  millimols  KCl  in  100  cc. 
tion. 

of  the  solu- 

G 

KCl 

Sp.  gr. 

0 
13.28 
25.98 
45.36 
54.23 
83.84 
100 

424.5 
383.4 
339.3 
271.4 
238.5 
149.0 
110.6 

1.1800 
1.1848 
1.1935 
1.2106 
1.2189 
1.2590 
1.2860 

Upper  layer  contains  per  100  g.  of  solution 

G.  H2O 

G.  acetone 

G.  KCl 

55.20 
54.27 
53.27 
51.69 
51.23 
50.34 
49.08 
48.02 
47.62 
46.49 
45.65 
45.64 
58.99 

31.82 
36.69 
35.44 
37.76 
48.50 
39.88 
41.67 
43.18 
43.73 
45.34 
46.52 
46.57 
25.24 

12.99 
12.03 
11.29 
10.55 
10.27 
9.77 
9.26 
8.79 
8.64 
8.17 
7.83 
7.79 
15.77 

(Herz  and  Knoch,  Z.  anorg.  1905,  45.  267.) 

Insol.    in    CS2.      (Baeyer;    Arctowski,    Z. 
anorg.  1894,  6.  257.) 
Insol.  in  benzonitrile.    (Naumann,  B.  1914, 
47.  1370.) 
Insol.  in  methyl  acetate.     (Naumann,  B. 
1909,  42.  3790);  ethy  1  acetate.     (Naumann, 
B.  1910,  43.  314.) 

Solubility  of  KCl  in  organic  compounds  +Aq 
i                                 at  25°. 

Lower  layer  contains  per  100  g.  of  solution 

G.  H<X) 

G.  acetone 

G.  KCl 

28.14 
29.45 
30.96 
31.83 
32.64 
34.07 
35.27 
37.44 
38.00 
38.68 
39.98 
40.41 
23.66 

69.42 
67.83 
65.97 
64.83 
63.79 
62.01 
i60.49 
:57.67 
56.96      i 
56.17 
54.36 
:53.78 
74.91 

2.44 
2.72 
3:.  07 
3.33 
3.56 
3.92 
4124 
4.89 
5.04 
5.25 
5.66 
5.81 
1.43 

Compound 

G.  comp. 
per  1.  H20 

G.  KCl  per 

100  g.  sat. 
solution 

Water 
Acetaldehyde 
Paraldehyde 
Glycerol 

Glycol 

ii 

Mannitol 
a 

ii.'oi 

11.07 
13.01' 
15.51 
62.05 
45.53 
136.59 

26.89 
27.05 
26.42 
25.58 
26.43 
25.26 
24.86 
24  .46 

(Armstrong  and  Eyre,  Proc. 
A,  88.  234.) 

Roy.  Soc.  1913, 

(Snell,) 

POTASSIUM  URANYL  CHLORIDE  , 


759 


Solubility  in  pyridine+Aq  at  10°. 

Potassium  thorium  chloride,  KC1,  2ThCl4+ 

Solvent 

100  g.  of  the 
solution  contain 

Deliquescent;    sol.    in   H2O    and    alcohol. 

H20 

Pyridine 

g.  KC1 

(Berzelius.) 

100 

0 

23.79 

Potassium  tin  (stannous)  chloride  (Potassium 

90 

10 

19.76 

chlorostannite),  KC1,  SnCl2+H2O.          i 

80 
70 

20 
30 

-16.37 
13.19 

Decomp.  by  H2O;  sol.  in  hot  HC1  or  KC1+ 
Aq.     (Remsen  and  Richardson,  Am.  Ch.  J. 

60 

40 

10.05 

14.  90.) 

50 
40 
30 

50 
60 
70 

6.34 
3.335 

2KC1,  SnCl2+H2O.    Partially  decomp.  by 
dissolving  in  H2O.    (Rammelsberg,  Pogg.  94. 

507.) 

20 
10 

80 
90   ' 

1  f\f\ 

0.'24 
0.039 

+2H2O.    Very  sol.  in  hot,  and  but  slightly 
in  cold  HCl+Aq  or  KCl+Aq.    (Remsen  and 

100 

Richardson.) 

(Schroeder,  J.  pr.  1908,  (2)  77.  268.) 

4KC1,  SnCl2+3H2O.    (Poggiale,  C.  R.  20. 

1182.) 

Tnsnl     in    sinnvrlrr»ii«   nvrirlinA   anH    in    Q7P/1 

Does  not  exist.    (Remsen  and  Richardson.) 

Jfe 

pyridine+Aq. 

Very  si.  sol.  in  95%  pyridine+Aq. 

SI.  sol.  in  93%  pyridine+Aq.  (Kahlen- 
berg,  J.  Am.  Chem.  Soc.  1908,  30.  1107.) 

100  ccm.  of  a  sat.  solution  of  KC1  in  fur- 
furol  at  25°  contain  0.085  pts.  by  wt.  KC1. 
(Walden,  Z.  phys.  Ch.  1906,  55.  713.) 

100  g.  H2O  dissolve  246.5  g.  sugar +44.8  g. 
KC1  at  31.25°;  100  g.  sat.  solution  contain 
62.28  g.  sugar+11.33  g.  KC1.  (Kohler,  Z. 
Ver.  Zuckerind,  1897,  47.  447.) 

Solubility  in  glucose +Aq  at  25°. 


Concentration  of 
glucose  in  9.  mol. 
per  1000  g  H20 

Solubility  in 
1000  g.  H2O 

Molecular 
solubility 

362.70 

4.86 

0.25 

366.10 

4.91 

0.50 

369.85 

4.96 

1.0 

376.25 

5.04 

3.0     . 

402.25 

5.39 

(Armstrong  and  Eyre,  Proc.  Roy.  Soc.  1910, 
84.  127.) 

Potassium  manganic  chloride,  K2MnCl5. 

Sol.  in  H2O;  less  sol.  in  NH4Cl+Aq;  un- 
stable.   (Neuman,  M.  1894,  15.  492.) 

Potassium  rhodium  chloride. 
See  Chlororhodite,  potassium. 

Potassium  ruthenium  sesg^ichloride. 
See  Chlororuthenite,  potassium. 

Potassium  ruthenium  ^rachloride. 
See  Chlororuthenate,  potassium. 

Potassium  tellurium  chloride. 
'See  Chlorotellurate,  potassium. 

Potassium   thallic   chloride,   3KQ1,   T1C18+ 

2H2O. 

Sol.  in  H2O.    Not  decomp.  by  boiling  H2O. 
(Rammelsberg.) 


Potassium  tin  (stannic)  chloride,  2KC1,  SnCl4. 
See  Chlorostannate,  potassium. 

Potassium  tungsten  chloride,  K2(OH)WC15. 

Decomp.  by  moisture.  Insol.  in  organic 
solvents.  (Olsson,  B.  1913,  46.  581.) 

K3W2C19.  Sol.  in  H2O.  Nearly  insol.  in 
most  organic  solvents.  (Olsson.) 

Potassium  uranium  chloride,  UC14,  2KC1. 

Very  hydroscopic;  sol.  in  H2O  with  decomp. ; 
sol.  in  acetic  acid.  Decomp.  by  alcohol. 
Nearly  insol.  in  ether.  (Aloy,  Bull.  Soc.  1899, 
(3)  21.  264.) 

Potassium  uranyl  chloride,  K2(UO2)C14. 

Very  sol.  in  H2O.  Moderately  sol.  in  dil. 
alcohol.  (Aloy,  Dissert.  1901.) 

+2H2O.  Very  sol.  in  H20  and  alcohol. 
(Arfvedson.) 

Sol.  in  H2O,  with  decomp.  and  separation 
of  KC1,  unless  H2O  is  acidulated  with  HC1. 
(Peligot,  A.  ch.  (3)  ;6.  37.)  / 

Solubility  in  H2O  at  t°. 


t° 

100  pts.  of  the  solution 
contain 

Solid  phase 

PtS; 

U02 

Pts. 
Cl 

Pts. 
K 

0.8 

14.9 
17.5 
25.0 
41.5 
50.0 
60.0 
71.5 
78.5 

38.57 

33.71 
37.36 
35.01 
35.27 
34.18 
34.19 
33.55 
35.26 

13.59 

13.51 
14.50 
15.26 
15.92 
16.56 
17.25 
17.44 
18.24 

3.86 

5^27 
7.'  39 

9.'i4 
9.28 
9.95 

UOzClj,  2KC1,  2H2O 
+KC1 

UOiCls,  2KC1,  2H2O 

(Rimbach,  B.  1904,  37.  463.) 

760 


POTASSIUM  VANADIUM  CHLORIDE 


Potassium  uranyl  chloride  is  decomp.  by 
H2O  at  temp,  below  60°.  Above  60°,  it  is 
sol.  in  H2O  without  decomp. 

Potassium  vanadium  chloride,  VK2C15+H2O. 
Difficultly  sol.  in  H2O  and  alcohol.    (Stab- 
ler, B.  1904,  37.  4412.) 

Potassium  yttrium  chloride. 

Sol.  in  H2O  with  evolution  of  heat. 

Potassium  zinc  chloride,  2KC1,  ZnCl2. 

Very  deliquescent.  Sol.  in  1  pt.  cold,  and 
in  all  proportions  of  hot  H2O.  (Pierre,  A.  ch. 
(3)  16.  248.) 

-fH2O.  Not  very  deliquescent.  Can  be 
recryst.  (Ephraim,  Z.  anorg.  1908,  69.  58.) 

KC1,  ZnCl2+2H2O.  Not  deliquescent. 
Cannot  be  recryst.  without  decomp. 
(Ephraim.) 

Potassium  chloroiodide,  KC12I. 

Very  unstable.  (Wells  and  Wheeler,  Sill. 
Am.  J.  143.  475.) 

KC14I.  Sol.  in  H2O  with  decomp.  Ether 
dissolves  out  IC13.  (Filhol,  J.  Pharm.  25. 
433.) 

Potassium  fluoride,  KF  or  K2F2. 

Very  deliquescent.  Very  sol.  in  H2O.  SI. 
sol.  in  HF+Aq.  Easily  sol.  in  cone.  KC2H3O2 
+Aq.  Insol.  in  alcohol.  (Berzelius.)  Sol. 
in  dilute  alcohol.  (Stromeyer,  A.  100.  83.) 

Sp.  gr.  of  aqueous  solution  of  KF  at  18° 
containing — 

5  10  20  30  40%  KF. 

1.041       1.084      1.117      1.272      1.378 
(Kohlrausch,  W.  Ann.  1879.  1.) 

Solubility  in  HF+Aq  at  21°. 
(G.  per  100  g.  H2O.) 


(Ditte,  C.  R.  1896, 123.  1282.) 

Easily  sol.  in  liquid  HF.  (Franklin,  Z 
.-anorg.  1905,  46.  2.) 

Very  si.  sol.  in  liquid  NH3.  (Gore,  Am.  Ch 
J.  1898,  20.  829.) 

Insol.  in  methyl  acetate.  (Naumann,  B 
1909,  42.  3790.) 


G.  KF 

G.  H2O 

G. 

acetone 

G.  KF 

G.  H20 

G. 

acetone 

5.75 

58.91 

35.34 

0.61 

31.95 

67.44 

5.00 

56.28 

38.72 

0.50 

29.92 

69.58 

3.84 

52.25 

43.91 

28.42 

69.76 

1.82 

3.06 

49.05 

47.89 

25.74 

71.24 

3.02 

2.61 

46.84 

50.55 

22.35 

72.99 

4.66 

2.22 

44.79 

52.99 

20.28 

73.80 

5.90 

14.95 

73.66 

11.39 

18.71 

74.10 

7.19 

11.46 

70.77 

17.77 

16.31 

73.97 

9.72 

9.17 

67.30 

23.53 

12.40 

72.01 

15.59 

7.72 

64.01 

28.27 

33.86 

65.73 

0.397 

7.07 

62.03 

30.90 

29.97 

68.54 

1.50 

6.43 

60.50 

33.07 

22.05 

73.41 

4.54 

1.38 

40.55 

58.06 

17.82 

74.01 

8.16 

0.979 

36.42 

62.60 

14.34 

73.29 

12.37 

0.693 

32.69 

66.61 

44.24 

55.52 

0.240 

0.57 

31.50 

67.93 

33.34 

65.66 

1.00 

0.89 

35.74 

63.36 

29.86 

68.54 

1.60 

0.75 

33.84 

65.41 

24.38 

72.16 

3.45 

HF 

KF 

HF 

KF 

0.0 

96.3 

13.95 

31.4 

1.21 

72.0 

15.98 

33.4 

1.61 

61.0 

17.69 

35.6 

3.73 

40.4 

20.68 

38.4 

4.03 

32.5 

28.60 

46.9 

6.05 

30.4 

41.98 

61.8 

9.25 

29.9 

53.71 

74.8 

11.36 

29.6 

74.20 

105.0 

12.50 

30.5 

119.20 

169.5 

KF  will  "salt  out"  acetone  from  aqueous 
solution.  The  table  shows  the  composi- 
tion of  the  solutions  at  the  points  at 
which  inhomogeneous  solutions  of  KF, 
acetone  and  H2O  just  become  homo- 
geneous at  20°. 
100  g.  of  the  solution  contain: 


At  the  first  quadruple  point  where  the 
hydrate,  acetone,  water  and  vapor  are  in 
equilibrium  the  upper  layer  contains  98% 
acetone,  while  the  lower  layer  contains  in 
100  g.,  46.3  g.  KF.  A  sat.  "solution  of  KF 
will  thus  dehydrate  acetone  to  the  extent  of 
98%. 

(Frankforter  and  Cohen,  J.  Am.  Chem.  Soc. 
1914,  36.  1115.) 

Similar  data  are  given  for  KF  in  ethyl  and 
propyl  alcohol  by  Frankforter  and  Frary. 
(J.  phys.  Ch.  1913,  17.  402.) 

+2H2O.  Very  deliquescent.  (Guntz,  A. 
ch.  (6)  3.  20.) 

Sat.  aq.  solution  at  18°  contains  45.3% 
KF  (de  Forcrand,  C.  R.  1911, 162. 1210.) 

Sp.  gr.  of  solution  sat.  at  18°  =  1.502,  and 
contains  48%  KF.  (Mylius  and  Funk,  B. 
1897,  30.  1718.) 

+4H2O.  Not  deliquescent,  (de  Forcrand, 
C.  R.  1911,  152.  1075.) 

Sat.  aq.  solution  at  18°  contains  35.96% 
KF.  (de  Forcrand,  C.  R.  1911,  162.  1210.) 

Potassium  hydrogen  fluoride,  KF,  HF  = 
KHF2. 

Easily  sol.  in  H2O.  SI.  sol.  in  H2O  con- 
taining HF.  Easily  sol.  in  cone.  KC2H3O2  + 
Aq.  Sol.  in  dil.  alcohol,  but  insol.  in  absolute 
alcohol. 

KF,  2HF.  Deliquescent.  Decomp.  by 
H2O  with  absorption  of  heat.  (Moissan,  C.  R. 
106.  547.) 

KF,  3HF.    As  above.    (Moissan.) 


POTASSIUM  HYDROXIDE 


761 


Potassium  manganic  fluoride. 
See  Fluomanganate,  potassium. 

Potassium  scandium  fluoride,  K3ScFe. 

Sol.  in  H2O.  Decomp.  by  acids.  (R.  J. 
Meyer,  Z.  anorg.  1914,  86.  275.) 

Potassium  silicon  fluoride. 
See  Fluosilicate,  potassium. 

Potassium  tantalum  fluoride. 
See  Fluotantalate,  potassium. 

Potassium  tellurium  fluoride,  KF,  TeF4. 

Decomp.  by  H2O.  (Hogbom,  Bull.  Soc. 
(2)  35.  60.) 

Potassium  thallic  fluoride,  2T1F3,  KF. 

Decomp.  by  moisture.  Insol.  in  HF. 
(Gewecke,  A.  1909,  366.  226.) 

Potassium  thorium  fluoride,  2KF,  ThF4-f 

4H20. 

Nearly  insol.  in  H2O.    Sol.  in  HF+Aq. 
KF,  ThF4.    Precipitate.    (Chydenius.) 

Potassium    tin    (stannous)    fluoride,    2KF, 

3SnF2+H2O. 
Sol.  in  H2O.    (Wagner,  B.  19.  896.) 

Potassium  tin  (stannic)  fluoride. 
See  Fluostannate,  potassium. 

Potassium  titanium  ^rafluoride. 
See  Fluotitanate,  potassium. 

Potassium  titanium  sesgiufluoride,  4KF, 
Ti2F6. 

Precipitate.  Very  si.  sol.  in  H2O.  Sol.  in 
dil.  acids.  (Piccini,  C.  R.  97.  1064.) 

See  also  Fluosesgm'titanate,  potassium. 

Potassium  titanyl  fluoride. 

See  Fluoxypertitanate,  potassium. 

Potassium  tungstyl  fluoride. 
See  Fluoxytungstate,  potassium. 

Potassium  uranium  fluoride,  KF,  UF4. 

Insol.  in  H2O  and  dil.  acids.  Difficultly 
sol.  in  cone.  HCl+Aq.  Sol.  in  cone.  H2SO4. 
(Bolton,  J.  B.  1866.  212.) 

Potassium  uranyl  fluoride. 
See  Fluoxyuranate,  potassium. 

Potassium  vanadium  sesquifluoride. 
See  Fluovanadate,  potassium. 

Potassium  vanadium  ^rcrfluoride  (?). 

Easily  sol.  in  H2O.  Insol.  in  alcohol. 
(Berzelius.) 


Potassium  zinc  fluoride,  KF,  ZnF2. 
Sol.  in  H2O.    (R.  Wagner.) 
2KF,  ZnF2.    Sol.  in  H2O.    (Berzelius.) 

Potassium  zirconium  fluoride. 
See  Fluozirconate,  potassium. 

Potassium  fluoride  hydrogen  peroxide,  KF, 

H202. 

Not  hydroscopic.  Very  sol.  in  H2O.  Is 
not  decomp.  at  70°  and  only  partially  so  at 
110°.  (Tanatar,  Z.  anorg.  1901,  28.  255.) 

Potassium  fluoride  vanadic  acid. 
See  Fluoxyvanadate,  potassium. 

Potassium  hydride,  KH. 

Decomp.  by  H2O.  Insol.  in  oil  of  tur- 
pentine, benzene,  ether  and  CS2.  (Moissan, 
C.  R.  1902,  134.  18.) 

Potassium  hydrosulphide,  KSH. 

Very  deliquescent,  and  sol.  in  H2O  with 
gradual  decomp.  Crystallizes  with  >£H2O. 
Sol.  in  alcohol. 

Potassium  hydroxide,  KOH. 

Very  deliquescent,  and  sol.  in  H2O  with 
evolution  of  much  heat.  100  pts.  KOH,  ex- 
posed over  H2O  at  16-20°  take  up  460  pts. 
H2O  in  56  days.  (Mulder.) 

1  pt.  KOH  dissolves  in  0.5  pt.  cold  H2O  (Lowitz) ; 
in  0.47  pt.  cold  H2O  (Bineau,  C.  R.  41.  509) ;  in  1  pt. 
H20.  (Abl.) 

Solubility  of  KOH  in  H2O  at  t°. 


t° 

G.  KOH  per  100  g. 

Solid  phase 

H2O 

solution 

—22 

3.7 

3.6 

Ice 

—20.7 

22.5 

18.4 

" 

—65.2 

44.5 

30.8 

" 

—36.2 

36.2 

26.6 

KOH.4H2O 

—32.7 

77.94 

43.8 

" 

—33 

80 

44.4 

KOH.4H2O+KOH. 

2H2O 

—23.2 

85 

45.9 

KOH.2H2O 

0 

97 

49.2 

" 

10 

103 

50.7 

" 

15 

107 

51.7 

" 

20 

112 

52.8 

" 

30 

126 

55.76 

" 

32.5 

135 

57.44 

KOH.2H20+KOH. 

H2O 

50 

140 

58.33 

KOH.H2O 

100 

178 

64.03 

" 

125 

213 

68.06 

" 

143 

311.7 

75.73 

(Pickering,  Chem.  Soc.  1893,  63.  908.) 

100  pts.  KOH  are  sol.  in  93.4  pts.  H2O  at 
15°  or  100  pts.  H2O  dissolve  107  pts.  KOH  at 
15°".  Sp.  gr.  =  1.5355  at  15°. 


762 


POTASSIUM  HYDROXIDE 


All  higher  values  found  in  solubility  tables 
are  incorrect.  (Ferchland,  Z.  anorg.  1902 
30.  133.) 

100  g.  sat.  aq.  solution  at  15°  contain 
50.48  g.  KOH.  (de  Forcrand,  C.  R.  1909, 
149.  719.) 

Sat.  KOH+Aq  boils  at  157.7°  (Griffiths) 
340°.  (Gerlach). 

B.-pt.  of  KOH+Aq  containing  pts.  KOH  tc 
100  pts.  H2O. 


B.-pt. 


105C 

110 

115 

120 

125 

130 

135 

140 

145 

150 

155 

160 

165 

170 

175 

180 

185 

190 

195 

200 

205 

210 


Pts.  KOH 


20.5 

34.5 

46.25 

57.5 

67.5 

76.8 

85.0 

92.5 

99.8 

106.5 

114.05 

121.7 

129.35 

137.0 

144.8 

152.6 

160.4 

168.2 

176.5 

185.0 

193.5 

202.0 


B.-pt. 


215° 

220 

225 

230 

235 

240 

245 

250 

255 

260 

265 

270 

275 

280 

285 

290 

295 

300 

310 

320 

33C 

340 


Pts.  KOH 


210.5 
219.8 
230.0 
240.9 
251.9 
263.1 
274.4 
285.7 
298.5 
312.5 
328.0 
343.5 
359.0 
375.0 
391.0 
408.2 
425.5 
444.4 
484.0 
526.3 
571.5 
623.6 


(Gerlach,  Z.  anal.  26.  464.) 


Sp.   gr.   and   b-pt.   of   KOH-f-Aq   according   to 
Dalton. 


%  K20 

Sp.  gr. 

B.-pt. 

%K2p 

Sp.  gr. 

B.-pt. 

4.7 

1.06 

100.56° 

36.8 

1.44 

123.89° 

9.5 

.11 

101  .  11 

39.6 

1.47  i 

129.44 

13.0 

.15 

101.66 

42.9 

1.52 

135.56 

16.2 

.19 

103.33 

46.7 

1.60 

143.33 

19.5 

.23 

104.44 

51.2 

1.68  ; 

160  .  00 

23.4 

.28 

106.66 

56.8 

1.78  , 

188  .  22 

26.3 

.33 

109.44 

63.6 

1.88  : 

215.56 

29.4 

.36 

112.22 

72.4 

2.00 

315.56 

32.4 

.39 

115.56 

84.0 

2.2     i 

red  heat 

34.4 

.42 

118.89 

100 

2.4. 

Sp.  gr.  of  KOH  +Aq  at  15°. 


%K20 

Sp.  gr. 

%  K?0 

Sp.  gr. 

%  K2d> 

Sp.  gr. 

0.568 

1.0050 

10.750 

1  .  1059 

20.935 

.2268 

1.697 

1.0153 

11.882 

1.1182 

21.500 

.2342 

2.829 

1.0560 

13.013 

1  .  13Q8 

22  .  632 

.2493 

3.961 

1.0369 

14.145 

1  .  1437 

23  .  764 

.2648 

5  .  002 

1.0478 

15.277 

1.1568 

24  .  895 

.2805 

6.224 

1  .  0589 

16.408 

1  .  1702 

26.027 

.2966 

7.355 

1.0703 

17.540 

1  .  1839 

27.158 

1.3131 

8.487 

1.0819 

18.671 

1  .  1979 

28  .  290 

1  .  3300 

9.619 

1.0938 

19  .  803 

1.2122 

(Zimmerman,  N.  J.  Pharm.  18,  2.  5. 


Sp.  gr.  of  KOH  +  Aq. 


%K20 

Sp.  gr. 

%  K20 

Sp.  gr. 

%  K?0 

Sp.  gr. 

2.44 

1.02 

23.14 

1.22 

37.97 

1.42 

4.77 

1.04 

24.77 

1.24 

40.17 

1.44 

7.02 

1.06 

26.34 

1.26 

42.31 

1.46 

9.20 

1.08 

27.86 

1.28 

44.40 

1.48 

11.28 

1.10 

29.34 

1.30 

46.45 

1.50 

13.30 

1.12 

30.74 

1.32 

48.46 

1.52 

15.38 

1.14 

32.14 

1.34 

50.09 

1.54 

17.40 

1.16 

33.46 

1.36 

51.58 

1.56 

19.34 

1.18 

34.74 

1.38 

53.06 

1.58 

21.25 

1.20 

35.99 

1.40 

(Richter.) 


Sp.  gr.  of  KOH  +Aq  at  15°.    a  = 
K2O;b  =  sp.  gr.  if  %  is 


% 


i 

2 
3 
4 
5 
6 
7 
8 
9 

10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 


.010 
.020 
.030 
.039 
.048 
.058 
.068 
.078 
.089 
.099 
.110 
.121 
.132 
.143 
.154 
.166 
.178 
.190 
.202 
.215 
230 
242 
256 
270 
285 
300 
312 
326 
340 
1.355 


.009 

.017 

.025 

.033 

.041 

.049 

.058 

.065 

.074 

.083 

.092 

.110 

.111 

.119 

.128 

.137 

.146 

1.155 

1.166 

1.177 

1.188 

1.198 

1.209 

1.220 

1.230 

1.241 

1.252 

1.264 

1.278 

1.288 


31 
32 
33 
34 
35 
36 
37 
38 
39 
40 
41 
42 
43 
44 
45 
46 
47 
48 
49 
50 
51 
52 
53 
54 
55 
56 
57 
58 
59 
60 


1.370 
1.385 
1.403 
1.418 
1.431 


445 

460 

475 

490 

504 

522 

539 

564 

570 

584 

600 

615 

630 

645 

660 

676 

690 

705 

1.720 

1.733 

1.746 

1.762 

1.780 

1.795 

1.810 


(Calculated  by  Gerlach,  Z.  anal.  8.  279, 
after  Zimmermann,  N.  J.  Pharm.  18,  2.  5,  ana 
Schiff,  A.  107.  300.) 


Sp.gr.  of  KOH+Aq  at  15°. 


%KOH 


4.2 

8.4 

12.6 

16.8 


Sp.  gr. 


1.0382 
1.0776 
1.1177 
1 . 1588 


%  KOH 


21.0 
25.2 
29.4 


Sp.  gr. 


1.2008 
1.2439 
1.2880 


(Kohlrausch,  W.  Ann.  1879.  1.) 


POTASSIUM  HYDROXIDE 


763 


Sp.gr.  of  KOH+Aqat  15°. 

Sp.  gr.  of  KOH+Aq. 
%  KOH                     6.87 
Sp.  gr.  20°/20°         1.0601 
(Le  Blanc  and  Rohland, 
19.  272 

KOH4-Aa  containing 

12.10 
1.1025 
Z.  phys.  Ch. 

eoual  nts.  of 

1896, 
KOH 

%  KOH 

Sp.  gr. 

%  KOH 

Sp.  gr. 

10 
20 
30 
40 

1.077 
1.175 

1.288 
1.411 

50 
60 
70 

1.539 
1.667 
1.790 

(Gerlach,  Z.  anal.  27.  275,  calculated  from 
Schiff,  A.  107.  300.) 


Sp.  gr.  of  K2O+Aq  at  15°. 


%K20 

Sp.  gr. 

%K20 

Sp.  gr. 

5 
10 
15 
20 
25 

1.054 
1.111 
1  .  171 
1.231 
1.294 

30 
35 
40 
45 

1.358 
1.428 
1.500 
1.576 

(Hager,  Adjumenta  varia,  Leipsic,  1876.) 


Sp.  gr.  of  KOH+Aq  at  20°  containing  2 
mols.  KOH  to  100  mols.  H2O  =  1.05325. 
(Nicol,  Phil.  Mag.  (5)  16.  122.) 

Sp.gr.  of  KOH+Aqat  15°. 


K§H 

Sp.gr. 

KO°H 

Sp.  gr. 

% 

KOH 

Sp.  gr. 

52 

1  .  53822 

34 

1.33313 

16 

1  .  14925 

51 

1.52622 

33 

1.32236 

15 

1  .  13955 

50 

1.51430 

32 

1.31166 

14 

1.12991 

49 

.50245 

31 

.30102 

13 

1.12031 

48 

.49067 

30 

.29046 

12 

1.11076 

47 

.47896 

29 

.27997 

11 

1.10127 

46 

.46733 

28 

.  26954 

10 

1.09183 

45 

.45577 

27 

.  25918 

9 

1.08240 

44 

.44429 

26 

1  .  24888 

8 

1.07302 

43 

.43289 

25 

1.23866 

7 

1.06371 

42 

.42150 

24 

1.22849 

6 

1.05443 

41 

.41025 

23 

1.21838 

5 

1.04517 

40 

.39906 

22 

1.20834 

4 

1.03593 

39 

.38793 

21 

1.19837 

3 

1.02671 

38 

.  37686 

20 

1  .  18839 

2 

1.01752 

37 

.  36586 

19 

1.17855 

1 

1.00834 

36 

1.35485 

18 

1  .  16875 

0 

0.99918 

35 

1.34396 

17 

1  .  15898 

(Pickering,  Phil.  Mag.  1894,  (5)  37.  375.) 

Sp.  gr.  of  N  solution  at  18°/4°  =  1.0481. 

(Loomis,  W.  Ann.  1896,  60.  550.) 

and  H2O  freeze^  at  — 54°.  (Guyton-Morveau, 
Gm.-K.  2,  1.  18.) 

KOH  is  completely  miscible  with  NaOH 
and  with  RbOH  in  both  the  liquid  and  the 
solid  states.  (Hevesy,  Z.  phys.  Ch.  1910,  73. 
667.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

Abundantly  sol.  in  strong  alcohol  or  wood- 
spirit. 

See  below  under  KOH+2H2O. 

Readily  sol.  in  glycerine. 

Sol.  in  not  less  than  25  pts.  of  ether. 
(Boullay .)  Sol.  in  much  more  than  25  pts.  of 
ether.  (Connell.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1904,37.3601.) 

Insol.  in  acetone.  Readily  sol.  in  fusel 
oil. 

Insol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014:) 

Sol.  in  aqueous  solution  of  mannite.  (Favre, 
A.  ch.  (3)  11.  76.) 

The  composition  of  the  hydrates  formed  by 
KOH  at  different  dilutions  is  calculated  from 
determinations  of  the  lowering  of  the  fr.-pt. 
produced  by  KOH  and  of  the  conductivity 
and  sp.  gr.  of  KOH+Aq.  (Jones,  Am.  Ch.  J. 
1905,  34.  337.) 

+H20. 

+2H2O.  Very  deliquescent,  and  sol.  in 
H2O  with  absorption  of  much  heat. 

100  g.  sat.  solution  in  H2O  at  30°  contain 
55.75  g.  anhyd.  KOH.  (de  Waal,  Dissert. 
1910.) 


Solubility  of  KOH+2H2O  in  alcohol+Aq'at 
30°. 


%  KOH 

%  alcohol 

%  HzO 

55.75 

0 

44.25 

54.81 

0.43 

44.76 

»  rf  • 

* 

31  'O 

57/50 

1150 

28.99 

65.07 

5.94 

27.67 

69.92 

2.41 

27.20 

73.01 

negative 

26.25 

81.98 

|t< 

*Separates  into  two  layers. 

(de  Waal,  Dissert,  1910.) 
+4H20. 


764 


POTASSIUM  HYDROGEN  TITANIUM  IMIDE 


Potassium  hydrogen  titanium  diimide, 

TS  (  TV  TT  MSI  K" 

Solubility  of  KI  in  100  pts.,  etc.  —  Continued. 

111  IN  -tLjIN-tY. 

Decomp.  by  H2O  and  alcohol.     Insol.  in 

t° 

Pts.  KI 

t° 

Pts.  KI 

t° 

Pts.  KI 

all  ord.  indifferent  organic  solvents.     (Ruff, 

57 

174 

78 

191 

99 

208 

B.  1912,  46.  1371.) 

58 

175 

79 

192 

100 

209 

•     59 

175 

80 

192 

101 

210 

60 

176 

81 

193 

102 

211 

Potassium  iodide,  KI. 

61 

177 

82 

194 

103 

212 

Deliquescent  only  in  very  moist  air.    Very 
sol.  in  H2O  with  absorption  of  heat. 
The  temp,  of  H2O  can  be  lowered  24°  by 
dissolving  KI.    (Baup.) 
140  pts.  KI  dissolved  in  100  pts.  H2O  at 
10.8°  lower  the  temp.  22.5°.    (Rtidorff,  Pogg. 
136.  276.) 

62 
63 
64 
65 
66 
67 
68 

178 
179 
180 
180 
181 
182 
183 

83 
84 

85 
86 
87 
88 
89 

195 
196 
197 
197 
198 
199 
200 

104 
105 
106 
107 
108 
109 
110 

213 
213 
214 
215 
216 
217 
218 

100  pts.  H2O  dissolve  126.6  pts.  KI  at  0° 
(Kremers);   127.8  pts.  KI  at  0°   (Mulder); 
127.9  pts.  KI  at  0°.     (Gerardin.) 
By  boiling,  100  pts.  H2O  dissolve  221  pts. 
KI  at  120°  (Baup);  222.2  pts.  KI  at  120° 
(Gay-Lussac);  222.6  pts.  KI  at  118.4°  (Mul- 
der); 223.58  pts.  KI  at  117°  (Legrand);  223.6 
pts.  KI  at  117°.     (Gerardin.) 
Between  these  temps,  the  solubility  in- 

69 
70 
71 

72 
73 
74 
75 
76 
77 

184 
184 
185 
186 
187 
188 
188 
189 
190 

90 
91 
92 
93 
94 
95 
96 
97 
98 

201 
202 
202 
203 
204 
205 
206 
207 
208 

111 
112 
113 
114 
115 
116 
117 

219 
220 
220 
221 
222 
223 
223.6 

creases  proportional  to  temp. 

(Mulder,  calculated  from  his  own  and  other 

Sr.1      in    O  73/i    r>t      TT.O    ot    1  9  Z°  •   \r>    O  7flQ    r>t      TToO    at. 

observations,  Scheik.  Verhandel.  1864.  63.) 

16°;  in  0.7  pt.  H2O  at    18°;   in  0.45  pt.  H2O  at  120°. 
(Graham-Otto.) 

100  pts.  KI+Aq  sat.  at  15-16°  contain  58.07  pts.  KI. 
(v.  Hauer,  J.  pr.  98,  137.) 


100  pts!  H2O  at  *12.5°  dissolve  136  pts.;  at  16°,  141 

OU1UULU.UJ    UJ.   -LVJ.  Ill   1\J\J  JJUO.   xx2vy   ai/   u    . 

pts.  KI.   (Baup.) 
100  pts.  H2O  at  18°  dissolve  143  pts.  KI;  at  120°,  271 
pts.     (Gay-Lussac.) 

t° 

Pts.  KI 

t° 

Pts.  KI 

t° 

Pts.  KI 

Sol.  in  0.79  pt.  H2O  at  0°;  in  0.70  pt.  H20  at  20°; 
in  0.63  pt.  H2O  at  48°;  in  0.57  pt.  H2O  at  60°;  in  0.53 
pt.  H2O  at  80°;  in  0.51  pt.  H2O  at  100°.     (Kremers, 
Pogg.  97.  15.) 

-22.65 
-22.35 
-16.8 

107.2 
106.6 
111.1 

21.05 
25.6 
29.1 

143.3 
146.6 
149.6 

71.1 
74.75 
81.6 

183.5 
185.6 
192.0 

-11.35 

116.3 

37.3 

156.7 

86.35 

194.6 

Sol.  in  0.71  pt.  H2O  at  15°.    CEder,  Dingl. 

991    8Q  ^ 

-5.9 
0 

120.4 
126.1 

42.3 
45.75 

160.3 
163.6 

93.5 
100.7 

200.3 
205.6 

AtfX*    Ot7.J 

+3.25 

130.1 

51.8 

167.6 

110.2 

216.1 

9.55 

134.0 

55.05 

169.1 

113.7 

218.8 

* 

12.75 

137.1 

60.55 

173.4 

Solubility  of  KI  in  100  pts.  H2O  at  t°. 

12.9 

137.9 

65.0 

178.3 

t° 

Pts.  KI 

t° 

Pts.  KI 

t° 

Pts.  KI 

(Coppet,  A.  ch.  (5)  30.  417.) 

0 

127.9 

19 

143.4 

38 

159 

1 

128.7 

20 

144.2 

39 

160 

2 

129.6 

21 

145.1 

40 

160 

Solubility  is  represented  by  a  straight  line 

3 

130.4 

22 

145.9 

41 

161 

of  the  formula  126.23  +0.8088t.    (Coppet.) 

4 

131.2 

23 

146.7 

42 

162 

5 

132.1 

24 

147.5 

43 

163 

6 

7 

132.9 
133.7 

25 

26 

148.3 
149.1 

44 
45 

164 
164 

Solubility  of  KI  in  100  pts.  H2O  at  high  temp. 

8 

134.5 

27 

149.9 

46 

165 

t° 

Pts.  KI 

t° 

Pts.  KI 

9 

135.3 

28 

150.7 

47 

166 

10 

136.1 

29 

151.5 

•48 

167 

124 

233.9 

144 

264.6 

11 

137.0 

30 

152.3 

49 

168 

133 

249.3 

175 

310.4 

12 

137.8 

31 

153 

50 

168 

13 

138.6 

32 

154 

51 

169 

(Tilden  and  Shenstone,  Phil.  Trans 

.  1884.  23.) 

14 

139.4 

33 

155 

52 

170 

15 

140.2 

34 

156 

53 

171 

16 
17 
18 

141.0 
141.8 
142.6 

35 
36 
37 

156 
157 
158 

54 
55 
56 

172 
172 
173 

If  solubility  S  =pts.  KI  in  100  pts.  solution, 
S  =  55.8+0.122t  from  0°  to   165°.      (fitard, 
C.  R.  98.  1432.) 

POTASSIUM  IODIDE 


765 


Sat. 

KI+Aq  contains  %  KI  at  t°. 

Sp.  gr.  of  KI+Aq  at  21°. 

ft 

1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 

Sp.  gr. 

% 

KI 

Sp.  gr. 

'& 

Sp.  gr. 

t° 

%  KI 

t° 

%KI 

-21 
-21 
-21 
-19 
-15 
-9 
0 
+21 
44 
72 

50.7 
51.0 
51.2 
52.2 
53.2 
54.5 
56.9 
59.3 
60.8 
64.3 

78 
96 
150 
151 
175 
176 
190 
193 
213 

64.8 
66.9 
70.6 
70.9 
71.6 
72.7 
73.8 
74.5 
75.7 

1.0075 
1.0151 
1.0227 
1.0305 
1.0384 
1.0464 
1.0545 
1.0627 
1.0710 
1.0793 
1.0877 
1.0962 
1.1048 
1.1136 
1  .  1226 
1.1318 
1.1412 
1.1508 
1  .  1605 
1  .  1705 

21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
34 
35 
36 
37 
38 
39 
40 

.1807 
.1911 
.2016 
.2122 
.2229 
1.2336 
1.2445 
1.2556 
1.2699 
1.2784 
1.2899 
1.3017 
1.3138 
1.3262 
.3389 
.3519 
.3653 
.3791 
.3933 
1.4079 

41 
42 
43 
44 
45 
46 
47 
.  48 
49 
50 
51 
52 
53 
54 
55 
56 
57 
58 
59 
60 

.4224 
.4371 
.4520 
.4671 
.4825 
.4982 
.5142 
.5305 
.5471 
.5640 
.5810 
.5984 
.6162 
.6343 
.6528 
.6717 
.6911 
.7109 
.7311 
.7517 

(fitard,  A.  ch.  1894,  (7)  2,  542.) 
Solubility  of  KI  in  100  g.  H2O  at  t°. 

t° 

g.KI 

t° 

g.KI. 

-1 
5 

122.2 
119.8 
117.4 
115.1 

75.8 

-11.5 
9  5 

64.7 
51.5 
42.6 
34.4 
25.7 

-4 
-10 
-14 

-7 
-6 
-5 

(Schiff,  A.  110.  75.) 

Sp.  gr.  cf  KI+Aq.    S  =  according  to  Schiff 
(A.  108.  340)  at  21°;  K  =  according  to  Kremers 
(Pogg.  96.  62),  interpolated  bv  Gerlach  (Z. 
anal.  8.  285.) 

(Meusser,  Z!  anorg.  1905,  44.  80.) 

102.70  pts.  by  weight  are  contained  in  100 
cc.  KI+Aq  sat.  at  25°,  or  59.54  pts.  in  100  g. 
of  solution;  sp.  gr.  =  1.7254. 
94.05  pts.  by  weight  are  contained  in  ICO  cc. 
KI+Aq  sat.  at  0°,  or  56.34  pts.  in  100  g.  of 
solution;  sp.  gr.  =  1.6699.     (Walden,  Z.  phys. 
Ch.  1906,  55.  715.) 

Solubility  of  KI  in  H2O  at  low  temperatures. 

5          10 
S    1.038  1.079 
K  1.038  1.078 

35        40 

S 

15        20 
1.123  1.171     . 
1.120  1.166  1 

45        50 
1  .483 

25 

..      ] 
218  ] 

55 

30%  KI, 
..279 
..271 

60%  KI. 

K  1.331   1.396  1.469  1.546  1.636  ] 
Sp.  gr.  of  KI+Aq  at  18°. 

.734 

g         Sp.  gr. 

& 

Sp.  gr. 

| 

Sp.  gr. 

t° 

%KI 

Solid  phase 

t° 

%  KI 

Solid  phase 

5      1.0363 
10      1.0762 
20      1  .  1679 

30 
40 
50 

1.273 
1.3966 
1.545 

55 

1.630 

-12.5 

IK 

38 
41.2 
44.6 
48 
51.2 
51.9 

Ice 
+KI 

-22 
20 

52.1 
52.6 
53.5 
54.5 
55.4 
56.4 

KI 
u 

It 
(( 
({ 
(I 

-17.5 
-20 
-22.5 

-15 
-10 
-  5 
0 

(Kohlrausch,  W.  Ann.  1879.  1.) 
Sp.  gr.  of  KI+Aq  at  18°. 

—23.2 

%KI 

Sp.  gr. 

(Kremann  and  Kershbaum,  Z.  anorg.  1907, 
56.  218.) 

1.044 
5.0 

1.0062 
1  .  0363 

149.26  g.  KI  dissolve  in  100  g.  H2O  at  25°. 
(Amadori  and  Pampanini,  Rend.  Ace.  Line. 
1911,  V,  20.  473.) 

60.39  g.  in  100  g.  KI+Aq  sat.  at  25°. 
(Parsons  and  Whittemore,  J.  Am.  Chem.  Soc. 
1911,  33.  1934.) 

56.1  g.  in  100  g.  KI+Aq  set.  at  0°;  60.35  g. 
in  100  g.  KI+Aq  sat.  at  30°.  (Van  Dam 
and  Donk,  Chem.  Weekbl.  1911,  8.  848.) 


(Giotrian,  W.  Ann.  1883,  18.  191.) 

Sp.  gr.  at  16°/4°  of  KI+Aq  containing 
32.4875%  KI  =  1.30238.  (Schonrock,  Z.  phys. 
Ch.  1893,  11.  781.) 

KI+Aq  containing  9.35%  KI  has  sp.  gr. 
20°/20°  =  1.0726. 

KI+Aq  containing  11.35%  KI  has  sp.  gr. 
20°/20°  =  1.0892.  '(Le  Blanc  and  Rohland,  Z. 
phys.  Ch.  1896,  19.  278.) 


766 


POTASSIUM  IODIDE 


B.-pt.  of  KI+Aq  containing  pts.  KI  to  100 
pts.  H2O. 

Sol.  in  liquid  SO2.     (Walden,  B.  1899,  32. 
2864.) 
Solubility  in  SO2  decreases  with  rise  of 
temp.    (Walden,  Z.  phys.  Ch.  1903,  42.  456.) 
Insol.  in  liquid  CO2.     (Biichner,  Z.  phys. 
Ch.  1906,  54.  674.) 
•  Very  easily  sol.  in  liquid  NH3.     (Franklin, 
Am.  Ch.  J.  1898,  20.  829.) 
Hydrazine  dissolves  135.7  pts.  KI  at  12.5- 
13°.    (de  Bruyn,  R.  t.  c.  1899,  18.  297.) 

100  pts.  alcohol  of  0.85  sp.  gr.  dissolve  18  pts.  KI 
at   12.5°.     100  pts.  absolute  alcohol  dissolve  2.5  pts. 

B.-pt. 

Pts.  KI 

B.-pt. 

Pts.  KI 

B.-pt. 

Pts.  KI 

101° 
102 
103 
104 
105 
106 
107 

15 
30 
45 
60 
74 
87 
99.5 

108° 
109 
110 
111 
112 
113 
114 

111.5 
123 
134 
145 
155 
165 
175 

115 
116 
117 
118 
118.5 

185° 
195 
205 
215 
220 

(Gerlach,  Z.  anal.  26.  439.) 


Sat.  KI+Aq  boils  at  H9°.    (Kremers.) 
Sat.  KI+Aq  forms  a  crust  at  117.5°,  and 
contains  210  pts.  KI  to  100  pts.  H2O;  highest 
temp,  observed,   118.5°.     (Gerlach,  Z.  anal. 
26.  426.) 


100  pts.  alcohol  of  D  sp.  gr.  at  0°  dissolve 
at  18°— 
D  0.9904  0.9851  0.9726  0.9665  0.9528 

130.5    119.4    100.1     89.9      76.9  pts.  KI, 

D  0.9390  0.9088  0.8464  0.8322 

66.4      48.2       11.4      6.2  pts.  KI. 


Solubility  of  KI  in  I2+Aq  at  25°. 


KI  mol./l. 

I  g.  -atoms/1. 

6.15 
6.23 
6.40 
6.36 
6.33 
6.24 

0.00 
3.64 
11.11 
13.16 
13.2 
17.03 

(Abegg,  Z.  anorg.  1906,  60.  428. 


Solubility  of  KI+I2  in  H2O  at  25°. 


a 

%l 

Solid 
phase 

| 

%l 

Solid 
phase 

29.45 
28.91 
26.84 
27.18 
27.14 

64.34 
63.88 
66.54 
67.14 
66.60 

KI+KI3 

if 

KI3+KI7 
it 

tt 

25.88 
25.57 
27.86 
27.27 
26.95 
25.71 

68.79 
69.01 
66.56 
66.91 
67.17 
67.91 

KI7+I2 

a 

KI3 

a 

KI7 
tt 

(Foote  and  Chalker,  Am.  Ch.  J.  1908,  39. 
564.) 

See  also  under  Iodine. 


KI+Aq  sat.  at  14.5°  containing  139.8  pts. 
KI  to  100  pts.  H2O  dissolves  1.0  pt.  K2S04 
with  separation  of  2.2  pts.  KI,  so  that  solution 
contains  137.6  pts.  KI  and  1.0  pt.  K2SO4  to 
100  pts.  H2O.  (Mulder,  Rotterdam,  1864.) 

100  pts.  H2O  dissolve  86.3  pts.  KI  and  2.1 
pts.  Na2SO4  at  14.5°.  (Mulder,  J.  B.  1866. 
67.) 

Sol.  in  AsCl3,  SnCl4  and  POC13.  (Walden, 
Z.  anorg.  19CO,  25.  21 4.) 

Attacked  by  dry  liquid  KO2  with  liberation 
of  I2.  (Frankland,  Chem.  Soc.  1901,  79.  1361 . 


That  is,  aqueous  alcohol  dissolves  approxi- 
mately the  same  amount  of  KI  that  the  water 
present  in  the  alcohol  would  dissolve,  and  it  is 
therefore  probable  that  KI  is  insol.  in  strictly 
absolute  alcohol.  (Gerardin.) 

Solubility  in  100  pts.  alcohol  of  0.9496  sp. 
gr.  at: 

8°       13°      25°      46°      55°      62° 
67.4     69.2     75.1     84.7     87.5     90.2  pts.  KI. 
(Gerardin,  A.  ch.  (4)  5.  155.) 


Sol.  in  68.3  pts.  absolute  alcohol  (Eder, 
Dingl.  221.  89);  in  370  pts.  ether  (sp.  gr. 
0.729),  (Eder,  I.e.);  in  120  pts.  alcohol-ether 
(1  : 1),  (Eder,  I.  c.) 

Sol.  in  10-12  pts.  90%  alcohol,  and  40  pts. 
absolute  alcohol.  (Hager,  Comm.  1883.) 

100  pts.  absolute  methyl  alcohol  dissolve 
16.5  pts.  at  20.5°;  100  pts.  absolute  ethyl 
alcohol  dissolve  1.75  pts.  at  20.5°.  (de  Bruyn, 
Z.  phys.  Ch.  10.  783.) 


Solubility  of  KI  in  methyl  alcohol +Aq  at  25 c 

p  =  %  by  wt.  of  alcohol  in  alcohol +Aq. 
S  =Sp.  gr.  of  alcohol+Aq  sat.  with  KI. 


L  =  millimols  KI  in 
tion. 


100  ccm.  of  the  solu- 


P 

S  25°/4° 

L 

0 

1.7213 

620 

10.6 

1.634 

555 

30.8 

1.460 

431 

47.1 

1.325 

335 

64.0 

1.185 

243 

78.1 

1.066 

169 

98.9 

0.9700 

113 

100 

0.9018 

.80 

(Herz  and  Anders,  Z.  anorg.  1907,  55.  274.) 


POTASSIUM  IODIDE 


767 


Solubility  of  KI  in  CH3OH. 

G  =  g.  KI  in  100  g.  of  the  solution, 
ti  =temp.  of  complete  solution. 
t2  =  temp,  at  which  salt  begins  to  separate 
out. 


Solubility  in  mixtures  of  methyl  and  propyl 
alcohol  at  25°. 

P  =  %  propyl  alcohol  in  the  solvent. 
G  =g.  KI  in  10  ccm.  of  the  solution. 
S  =Sp.  gr.  of  the  sat.  solution. 


G 

ti 

t2 

P 

G 

S  25°/4° 

8.64 
12.95 
14.2 
14.6 
14.97 
19.2 
26.8 
28.9 

"6° 

20 

25 
85 
115 
144 

266° 

262 

256 
242 
229 

0 
11.11 
23.8 
65.2 
91.8 
93.75 
100 

1.316 
1.096 
0.854 
0.262 
0.060 
0.058 
0.043 

0.9018 
0.8823 
0.8629 
0.8187 
0.8045 
0.8041 
0.8041 

29.6 

188 

196 

33.0 

(Herz  and  Kuhn.) 

(Centnerszwer,  Z,  phys.  Ch.  1910,  72.  432.) 
Solubility  of  KI  in  methyl  alcohol  at  t°. 


Solubility  in  mixtures  of  propyl  and  ethyl 
alcohol  at  25°. 


t° 

g.  KI  in  100 
g.  alcohol 

t° 

g.  Klin  100 
g.  alcohol 

y—/o  propyl  alconoi  in  tne  solvent. 
G  =  g.  KI  in  10  ccm.  of  the  solution. 
S  =  Sp.  gr.  of  the  sat.  solution. 

15 
30 
50 

80 
100 
120 
140 
160 

14.50 
16.20 
18.9 
22.5 
25.0 
27.2 
29.2 
30.6 

180 
200 
220 
240 
245 
247 
250 
252.5* 

30.7 
29.1 
27.5 
24.8 
22.6 
21.0 
13.8 
7.6 

p 

G 

S  25°/4° 

0 

8.1 
17.85 
56.6 
88.6 
91.2 
95.2 
100 

0.155 
0.146 
0.137 
0.075 
0.052 
0.049 
0.044 
0.043 

0.8015 
0.7983 
0.7991 
0.7988 
0.8022 
0.8027 
0.8029 
0.8041 

*Critical  temp,  of  solution. 
(Tyrer,  Chem.  Soc.  1910.  97.  626.) 

At  room  temp.  1  pt.  KI  by  weight  is  sol.  in 
6  pts.  methyl  alcohol  D15  0.7990. 
16    "    ethyl          "       D15  0.8322. 
219    "    propyl        "       D15  0.8160. 

(Rohland,  Z.  anorg.  1898,  18.  325.) 

Solubility  in  mixtures  of  methyl  and  ethyl 
alcohol  at  25°. 

P  =  %  methyl  alcohol  in  the  solvent. 
G  =g.  KI  in  10  ccm.  of  the  solution. 
S  =Sp.  gr.  of  the  sat.  solution  at  25°. 


P 

G 

S  25°/4° 

0.00 

0.155 

0.8015 

4.37 

0.191 

0.8041 

10.40 

0.225 

0.8071 

41.02 

0.494 

0.8295 

80.69 

1.013 

0.8794 

84.77 

1.072 

0.8795 

91.25 

1.184 

0.8908 

100.00 

1.316 

0.9018 

(Herz  and  Kuhn.) 


100  g.  methyl  alcohol  dissolve  18.04  g.  KI 
at  25°. 

100  g.  ethyl  alcohol  dissolve  2.16  g.  KI  at 
25°. 

100  g.  propyl  alcohol  dissolve  0.43  g.  KI 
at  25°. 

100  g.  isoamyl  alcohol  dissolve  0.09  g.  KI 
at  25°. 

(Turner  and  Bissett,  Chem.  Soc.  1913, 103. 
1909.) 


0.455  g.  is  sol.  in  100  g.  propyl  alcohol. 
Schlamp,  Z.  phys.  Ch.  1894,  14.  276.) 

Alcoholic  solution  can  be  mixed  with  ^  vol. 
ether  without  pptn. 

100  g.  95%  formic  acid  dissolve  38.2  g. 
KI  at  18.5°.  (Aschan,  Chem.  Ztg.  1913,  37. 
.113.) 


(Herz  and  Kuhn,  Z.  anorg.  1908,  60.  155.) 


768 


POTASSIUM  IODIDE 


Solubility  in  organic  solvents  at  t°. 

C  =  pts.  by  wt.  of  KI  in  100  ccm.  of  the 
sat.  solution. 

L  =  no.  of  litres  which  at  the  saturation 
temp,  hold  in  solution  1  mol.  KI. 

S  =  sp.  gr.  of  the  solution  at  t°,  referred  to 
H2O  at  t°. 

p  =  pts.  by  wt.  of  KI  in  100  g.  of  the  solu- 
tion. 


Solvent 

t° 

c 

L 

S 

p 

Water 

25° 

102.70 

0.162 

1.7254 

59.54 

0° 

94.05 

0.177 

1  .  6699 

56.32 

Methyl  alcohol 

25° 

13.48 

1.231 

0  .  9003 

14.97 

(* 

25° 

14.26 

" 

0° 

11.61 

1.430 

0.8964 

12^95 

Ethyl  alcohol 

25° 

1.520 

10.92 

0  .  7908 

1  .  922 

0° 

1.197 

13.87 

0.8085 

1.479 

Glycol 

25° 

45.85 

0  .  362  ) 

1  .  3888 

33.01 

" 

25° 

47.23 

0.351) 

" 

0° 

43.28 

0.383 

1  .  3954 

31^03 

Acetonitrile 

25° 

1.551 

10.70 

25° 

1.590 

10.44 

0.7936 

2^003 

' 

0° 

1.852 

9.00 

0.8198 

2.259 

Propiomtrile 

25° 

0.316 

52  .  53  ) 

0.7821 

0.404 

1 

25° 

0.355 

46.76V  ) 

' 

0° 

0.344 

48  .  26  )  V 

0.8005 

0^429 

0° 

0.412 

40.29     } 

Benzonitrile 

25° 

0.051 

325.5 

1  .  0076 

0^050 

Nitromethane 

25° 

0.349 

47.56 

1  .  1367 

0.307 

25° 

0.289 

57.44 

" 

0° 

0.366 

45.36 

1  .  1627 

0^315 

" 

0° 

0.314 

52.87 

Nitrobenzene 

25° 

0.0019 

87.40 

Acetone 

25° 

1.038 

16.0 

0.7968 

l'302 

0° 

1.732 

9.58 

0  .  8227 

2.105 

Furfurol 

25° 

5.93 

2.80 

1.2014 

4.94 

" 

0° 

15.10 

1.10 

Benzaldehyde 

25° 

0.343 

48.4 

1  .  0446 

0^328 

Salicy  laldehy  d  e 

25° 

0.549 

30.24 

1  .  1373 

0.483 

" 

0° 

1.257 

13.21 

1.1501 

1.093 

Anisaldehyde 

25° 

0.720 

23.06 

1.1180 

0.644 

" 

0° 

1.520 

10.92 

1  .  1223 

1.355 

Ethyl  acetate 
Methyl  cyan- 

25° 

0.0013 

12.80 

acetate 

25° 

2.459 

6.75 

1  .  1358 

2.165 

0° 

3.256 

5.10 

1.1521 

2.827 

Ethyl  cyan- 

acetate 

25° 

0.888 

18.7 

1  .  0579 

0.839 

25° 

1.090 

15.23 

1.0678 

1.021 

(Walden,  Z.  phys.  Ch.  1906,  65.  715.) 

Insol.  in  CS2.    (Arctowski,  Z.  anorg.  1894, 
6.  257.) 

Sol.  in  benzonitrile.     (Naumann,  B.  1914, 
47.  1369.) 

Difficultly  sol.  in  methyl  acetate.     (Nau- 
mann, B.  1909,  42.  3789.) 

Sol.  in  ethyl  acetate.     (Casaseca,  C.  R.  30. 
821.) 

Insol.   in   ethyl   acetate.      (Naumann,   B 
1910,  43.  314.) 

Insol.    in    ethylamine.      (Shinn,    J.    phys 
Chem.  1907,  11.  538.) 

100  pts.  acetone  dissolve  2.930  pts.  KI  at 
25°.    (Krug  and  M'Elroy,  J.  Anal.  Ch.  6. 184.) 

Sol.  in  acetone,  insol.  in  methylal.     (Eid- 
mann,  C.  C.  1899.  II.  1014.) 
3.08  pts.  sol.  in  100  pts.  acetone  at  —2.5°. 
2.38      "      "'   "  100      "        "         "  +22°. 
1.21      "      "   "  100      "        "         "     56°. 


0.26      "      "   "  100 
0.11      "      "   "  100 

(Laszczynski,   B.    1894,   27.   2287.) 


"  pyridine  "      10°. 
"        "          "    119°. 


Freely  sol.  in  glycerine.  Insol.  in  acetic 
acid.  (Berthemot.) 

Sol.  in  3  pts.  glycerine;  insol.  in  olive  oil. 

and  Garot.) 
100  g.  glycerol  dissolve  40  g.  KI  at  15.5°. 
Ossendowski,  Phann.  J.  1907,  79.  575.) 

Potassium  £riiodide,  KI3. 

Very  deliquescent;  very  sol.  in  H2O  and 
alcohol.  (Johnson,  Chem.  Soc.  1877,  1. 
249.) 

Solution  of  I  in  K  I  contains  this  salt  (see 
KI).  Decomp.  by  heat  or  shaking  with  CS2, 
ther,  chloroform.  Sol.  in  alcohol,  from 
which  CS2  does  not  remove  I.  (Jorgensen,  J. 
pr.  (2)  2.  247.) 

Potassium  periodide. 

Solubility  determinations  show  that  the 
compds.  KI3  and  KI7  are  the  only  periodides 
of  potassium  which  form  solids  at  25°. 

See  under  KI+I.  (Foote  and  Chafer, 
Am.  Ch.  J.  1908,  39.  566.) 

K17.     See  above. 

Potassium  mercuric  iodide  ammonia, 

K2HgI4,  2NH3. 
(Peters,'  Z.  anorp.  1912,  77.   188.) 

Potassium  silver  iodide,  KI,  Agl. 

Sol.  in  KI+Aq.  Sol.  in  hot  alcohol. 
(Boullay,  A..ch.  34.  377.) 

2KI,  Agl,  Sol.  in  KI+Aq.  Decomp.  by 
H2O  (Boullay.) 

Hygroscopic.  (Hellwig,  Z.  anorg.  1900,  25. 
180.) 

SKI,  Agl.  Decomp.  by  H2O.  (Ditte,  C.  R. 
93,  415.) 

KI,  2  Agl.  Sol.  in  methylethylketone. 
(Marsh,  Chem.  Soc.  1913,  103.  783.) 

Potassium  silver  polyiodide,  AgK3I12,  3KI  + 

5H2O. 

Very  deliquescent.  (Johnson,  Chem.  Soc. 
33.  183.) 

Potassium  tellurium  iodide. 
See  lodotellurate,  potassium. 

Potassium  thallic  iodide,  KI,  T1I3. 

Decomp.  by  H2O.  Can  be  crystallized  from 
alcohol.  (Willm.) 

SKI,  2T1I3+3H2O.  Partially  decomp.  by 
H2O.  (Rammelsberg.) 

Potassium  (tin)  stannous)  iodide,  KI,  SnI2  + 


When  treated  with  a  small  quantity  of  H2O, 
KI  dissolves  out;  but  when  more  H2O  is 
added,  the  substance  is  completely  dissolved. 
More  sol.  in  warm  than  cold  alcohol.  (Boul- 

lay.) 


POTASSIUM  SULPHIDE 


769 


Potassium  zinc  iodide,  KI,  ZnI2. 

Very  deliquescent.  (Rammelsberg,  Pogg 
43.  665.) 

K2ZnI4+2H2O.  Hydroscopic.  (Ephraim 
Z.  anorg.  1910,  67.  382.) 

Potassium  iodide  sulphur  dioxide,  KI,  SO2 
(Pochard,  C.  R.  1900,  130.  1188.) 
KI,  4SO2.     (Walden,  Z.  phys.  Ch.  1903 

42.  439.) 

KI,  14SO2.    fWalden.) 

Potassium  nitride,  K2N. 

Decomp.  violently  by  H2O.     (H.  Davy. 

Potassium  ruthenium  efoTiydronitrosobromide 

Ru2H2  NOBr3,  2HBr,  3KBr. 
Ppt.     (Brizard,  A.  ch.  1900,  (7)  21.  362.) 

Potassium  ruthenium  nitrosochloride, 

Ru2H2NOCl3,  3KC1,  2HC1. 
SI.  sol.  in  H2O.     (Brizard,  C.  R.  1899,  129 
216.) 

Potassium  sw&oxide. 

Decomposes  H2O. 

Does  not  exist.  (Lupton,  Chem.  Soc.  1876, 
2.  565.) 

Potassium  oxide,  K2O. 

Very  sol.  in  H2O  with  much  heat. 
See  Potassium  hydroxide. 

Potassium  dioxide,  K2O2. 

Deliquescent.    Sol.  in  H2O.  Wft 

Forms  compound  K2O2,  2H2O2.     (Schone. 

A.  193.  241.) 

Potassium  peroxide,  K2O4. 

Deliquescent.  Very  sol.  with  decomp.  in 
H20. 

Potassium  silicon  oxyfluoride,  SiF2(OK)2  and 

SiO(F)OK. 
(Schiff  and  Becjii,  A.  Suppl.  4.  33.) 

Potassium  tantalum  oxyfluoride,  K4Ta4O6F14. 
Insol.  in  boiling  water.    Easily  sol.  in  HF  + 
Aq.    (Marignac,  A.  ch.  (4)  9.  268.) 

Potassium  phosphide,  KP3. 

Decomp.  by  H2O.  (Joannis,  C.  C.  1894, 
II.  834.) 

KP5.  Easily  decomp.  by  H2O.  (Hugot, 
C.  R.  1895,  121.  208.) 

Potassium  hydrogen  phosphide,  PH2K. 

Decomp.  by  H2O.  (Joannis,  C.  R.  1894, 
119.  558.) 

Potassium    phosphoselenide,    KSeP  =  K2Se, 

P2Se. 

Sol.  in  cold  H2O  with  rapid  decomp.  Sol. 
in  alcohol  with  slight  decomp.  (Hahn,  J.  pr 
93.  430.) 


Potassium    phospho^nselenide,    2K2Se, 

P2Se3. 

Deliquescent.  Decomp.  violently  with  H2O. 
Sol.  in  alcohol  or  ether,  or  in  a  mixture  of  the 
two,  with  slight  decomp.,  but  decomp.  gradu- 
ally on  the  air.  (Hahn,  J.  pr.  93.  430.) 

Potassium  phosphopentoselenide,  K4P2Se7  = 

2K2Se,  P2Se5. 

Deliquescent;  immediately  decomp.  by 
H2O,  alcohol,  or  ether.  (Hahn.) 

Potassium  phosphosulphide,  4K2S2,  P2S3. 
Deliquescent.     Sol.  in  H2O  with  decomp. 

Potassium  selenide,  K2Se. 

Sol.  in  H2O  with  subsequent  decomp.  on  the 
air. 

Insol.  in  liquid  NH3;  sol.  in  air  free  H2O 
to  a  colorless  liquid.  (Hugot,  C.  R.  1899, 
129.  299.) 

+2H2O.  Sol.  in  H2O  with  decomp. 
(Clever,  Z.  anorg.  1895,  10.  143.) 

+9,  14,  or  19H2O.  (Fabre,  C.  R.  102. 
olo.) 

Potassium  te^raselenide,  K2Se4. 

Easily  sol.  in  H2O.    Decomp.  on  standing. 

Sol.  in  liquid  NH3.  (Hugot,  C.  R.  1899, 
129.  299.) 

Potassium  wonosulphide,  K2S. 

Deliquescent.  Sol.  in  H2O  and  alcohol. 
H2O  solution  decomp.  on  air. 

Sol.  in  10  pts.  glycerine.  (Cap  and  Garot, 
J.  Pharm.  (3)  26.  81.) 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  829.) 

Insol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

Insol.  in  methyl  acetate.     (Naumann.  B 
1909,  42.  3790.) 

+5H2O.     (Schone,  Pogg.  131.  380.) 

All  potassium  sulphides  are  sol.  in  glycerine; 
nsol.  in  ether  and  ethyl  acetate. 

Potassium  ^'sulphide,  K2S2. 

Sol.  in  H2O  and  alcohol,  with  gradual  de- 
omp. 

Potassium  Zn'sulphide,  K2S3. 

Sol.  in  H2O  and  alcohol,  with  gradual  de- 
onip.  on  the  air. 

Potassium  tefrasulphide,  K2S4. 
Sol.  in  H2O  and  alcohol. 
+2H2O.    Sol.  in  H2O.    SI.  sol.  in  alcohol. 
+8H2O.    Sol.  in  H2O.    Alcohol  takes  out 
rater.     (Schone.) 

Vrtassium  pentasulpbide,  K2S6. 
Sol.  in  H2O  and  alcohol. 


770 


POTASSIUM  PALLADIUM  SULPHIDE 


Potassium  palladium  sulphide. 
See  Sulphopalladate,  potassium. 

Potassium  platinum  sulphide. 
See  Sulphoplatinate,  potassium. 

Potassium  silver  sulphide, 

4Agr2S,  K2S+2H2O. 

Decomp.  by  H2O.  (Ditte,  C.  R.  1895,  120. 
91.) 

Potassium  rhodium  sulphide,  3K2S,  Rh2S3. 
Decomp.  by  H2O.     (Leidie\) 

Potassium  tellurium  sulphide. 
See  Sulphotellurate,  potassium. 

Potassium  thallium  sulphide,  K2S,  T12S3. 

Not  decomposed  by  H2O,  or  hot  NH4OH,  or 
KOH+Aq.  Decomp.  by  HC1  or  moderately 
cone.  H2S04+Aq.  Hot  HNO3+Aq  decomp. 
with  separation  of  S.  (Schneider,  J.  pr.  110. 
168.) 

Potassium  tin  (stannic)  sulphide. 
See  Sulphostannate,  potassium. 

Potassium  zinc  sulphide,  K2S,  3ZnS. 

Not  attacked  by  H2O,  but  easily  decomp. 
by  the  most  dil.  acids.  (Schneider,  J.  pr.  (2) 
8.  29.) 

Potassium  telluride,  K2Te. 

Sol.  in  H2O.  (Demargay,  Bull.  Soc.  (2) 
40.  99.) 

Sol.  in  H2O  and  liquid  NH3.  (Hugot,  C.  R. 
1899,  129.  388.) 

Praseocobaltic  chloride, 

Co(NH3)4Cl3+H20. 

Easily  sol.  in  H2O. 

Dil.  HCl-i-Aq  dissolves  traces;  cone.  HC1+ 
Aq  dissolves  more.  Sol.  in  NH4OH+Aq  with 
decomp.  Sol.  in  cone.  H2SO4  without  de- 
comp. SI.  sol.  in  dil.  H2SO4+Aq.  (Rose.) 

—  mercuric  chloride,  Co(NH3)4Cl3,  HgCl2. 
SI.  sol.  in  cold  H2O;  insol.  in  HgCl2+Aq. 
.(Vortmann,  B.  15.  1892.) 


chloride  bichromate, 

[CoCl2(NH3)4]2Cr2O7+H2O. 
Scarcely  sol.  in  cold,  'easily  sol.  in  warm 
W>.    (Vortmann,  B.  15.  1897.) 

;Praseocobaltic  chloride  nitrate, 

CoCl2(NH3)4N03+H20. 
Much  less  sol.  in  H2O  than  the  chloride. 
'Precipitated  from  aqueous  solution  by  dil. 
IHNOa+Aq.    (Vortmann,  B.  15.  1896.) 


Praseodymicotungstic  acid. 

Ammonium  praseodymicotungstate, 

2(NH4)2O,  Pr2O3,  16WO3  +  16H2O. 
Very  si.  sol.  in  H2O.     Decomp.  by  acids 
and  alkalies.     (E.  F.  Smith,  J.  Am.  Chem. 
Soc.  1904,  26.  1478.) 

Barium  praseodymicotungstate,  4BaO,  Pr203, 
16WO3+7H2O. 

Ppt.    Insol.  in  H2O. 

6BaO,  Pr2O3,  16WO3+9H2O.  Ppt.  (E.  F. 
Smith.) 

Silver  praseodymicotungstate,  4Ag2O,  Pr2O3, 

16WO3+8H2O. 
Insol.  in  H2O.    (E.  F.  Smith.) 

Praseodymium,  Pr. 

Praseodymium  bromide,  PrBr3+6H2O. 

Very  sol.  in  H2O;  sol.  in  HBr.  (von  Schule, 
Z.  anorg.  1898,  18.  353.) 

Praseodymium  carbide,  PrC2. 

Decomp.  by  H2O;  insol.  in  cone.  HNO3, 
decomp.  by  dil.  HNO3.  (Moissan,  C.  R. 
1900,  131.  597.) 

Praseodymium  chloride,  PrCl3. 

Very  sol.  in  H2O.  Insol.  in  PC13  or  SnCl4. 
Sol.  in  alcohol.  Insol.  in  ether  and  most  or- 
ganic solvents.  (Matignon,  C.  R.  1902,  134. 
427.) 

2.14  g.  PrCl3  dissolve  in  100  g.  pyridine  at 
15°.  (Matignon,  Int.  Cong.  App.  Cbem.  1909, 
2.  53.) 

+H20. 

+3H2O. 

+7H2O.  100  g.  H2O  dissolve  334.2  g. 
PrCl3+7H2O  or  103.9  g.  of  the  anhydrous 
salt  at  13°.  The  aqueous  solution  sat.  at 
14°  has  a  sp.  gr.  16716°  =  1.687.  At  100°,  the 
solubilitv  in  H2O  is  unlimited.  (Matignon, 
A.  ch.  1906,  (8)  8.  388.) 

Sol.  in  cone.  HC1.  (von  Schule,  Z.  anorg. 
1898,  18.  352.) 

100  pts.  of  a  solution  of  the  salt  in  HCl+Aq 
contain  at  13°,  41.05  pts.  of  anhydrous  salt 
and  7.25  pts.  HC1.  Sp.  gr.  of  this  solution  at 
16°  =  1.574.  (Matignon,  A.  ch.  1906,  (8)  8. 
388.) 

Praseodymium  hydride,  PrH3  (?). 
(Muthmann,  A.  1904,  331.  59.) 

Praseodymium  hydroxide. 

Sol.  in  citric  acid.  (Baskerville,  J.  Am. 
Chem.  Soc.  1904,  26.  49.) 

Praseodymium  nitride,  PrN. 

Decomp.  in  moist  air  with  evolution  of 
NH3.  (Muthmann,  A.  1904,  331.  59.) 


RADIUM  EMANATION 


771 


Praseodymium  oxide,  Pr2O3. 

Easily  sol.  in  H2O.  (v.  Welsbach,  M.  6. 
477.) 

Decomp.  by  heating  in  the  air.  (Scheele, 
Z.  anorg.  1898,  17.  322.) 

Praseodymium  raonoperoxide,  Pr(OH)2.H2O. 
(Melikoff,  Chem.  Soc.  1902,  82.  (2)  140.) 

Praseodymium  s?;pm>xide,  Pr(OH)2(OOH). 
Ppt.    (Melikoff,  C.  C.  1902,  I.  172.) 

Praseodymium  trisuperoxide,  Pr(OOH)3. 
Ppt.    (Melikoff.) 

Praseodymium  peroxide,  Pr4O7. 

Sol.  in  acids  with  evolution  of  O.  (v. 
Welsbach.) 

Praseodymium  oxy sulphide,  Pr2SO2. 
(Biltz,  Z.  anorg.  1911,  71.  436.) 

Praseodymium  ^'sulphide,  PrS2. 

Decomp.  by  heat.  (Biltz,  Z.  anorg.  1911, 
71.  437.) 

Purpureocobaltic  salts. 

For  other  purpureocobaltic  salts,  see — 
Chloropurpureocobaltic  salts. 
Bromopurpureocobaltic  salts. 
Nitratopurpureocobaltic  salts. 
Suiphatopurpureocobaltic  salts. 

Purpureocobaltic  cobalticyanide, 

Co(NH3)5Co(CN)6  +  l^H2O. 
Insol.  in  H2O. 

—  ferricyanide,  Co(NH3)5Fe(CN)6. 

Insol.  in  cold  H2O.  Probably  belongs  to 
roseo  series. 

mercuric  hydroxycbloride, 

CoN5Hu(HgCl)3(HgOH)Cl3. 

Ppt.  (Vortmann  and  Morgulis,  B.  22. 
2645.) 

CoN5Hn(HgOH)4Cl3.    Ppt.    (V.  and  M.) 

mercuriodide,  basic, 

Co^5Hn(HgI2)2(HgOH)3I3. 
Ppt.     SI.  sol.  in  acids.     Sol.  in  KI+Aq. 
(Vortmann  and  Borsbach,  B.  23.  2804.) 

^—  molybdate,  Co2O3(NH3)10,  7MoO3+ 

3H2O  (?). 

Insol.  in  H2O  or  dil.  HC2H3O2+Aq.  (Car- 
not,  C.  R.  109.  109.) 

— • — •  sulphate. 

See  Suiphatopurpureocobaltic  salts. 

tungstate,  Co(NH3)6O(WO4). 

Scarcely  sol.  in  cold  or  hot  H2O.    (Gibbs.) 
Co2O3(NH3)10,   10WO3+9H2O  (?).     Insol. 


in  H2O,  or  dil.  HC2H3O2+Aq,  or  NH4OH  + 
Aq.    (Carnot,  C.  R.  109.  147.) 

Purpureocobaltic    vanadate,     Co2O3(NH3)io, 

5V2O5+9H2O  (?). 

Ppt.  Insol.  in  H2O.  (Carnot,  C.  R.  109. 
147.) 

Purpureocobaltic  octamine  salts. 

See  Octamine  cobaltic  purpureo  salts. 
Pyrosulphuric  acid,  H2S2O7. 

See  Disulphuric  acid. 
Radium,  Ra. 
Radium  A. 

More  sol  than  Radium  B  and  C  in  all 
solvents;  sol.  even  in  organic  solvents,  espe- 
cially CS2.  (Ramstedt,  Le  Radium,  1913,  10. 
159.) 

Radium  B. 

More  quickly  sol.  than  Radium  C  in  H2O 
and  acids;  less  quickly  sol.  in  alkaline  solu- 
tions; very  si.  sol.  in  organic  solvents.  (Ram- 
stedt, Le  Radium,  1913,  10.  159.) 

Radium  C. 

Sol.  in  common  acids,  less  so  in  alkaline 
solutions  and  in  H2O,  only  very  si.  sol.  in 
organic  solvents.  (Ramstedt,  Le  Radium, 
1913,  10.  159;  Chem.  Soc.  1913,  104.  (2)  659.) 

Radium  bromide. 

Less  sol.  in  H2O  than  corresponding  Ba 
comp.  (Curie,  Dissert.  1903.) 

Radium  chloride. 

Less  sol.  in  H2O  than  corresponding  Ba 
coniD.  (Curie,  Dissert.  1903.) 

Radium  emanation. 

Coefficient  of  absorption  for  H2O  =0.245  at 
3°;  0.23  at  20°;  0.17  at  40°;  0.135  at  60°;  0.12 
at  70°;  0.12  at  80°.  (Hofmann,  Phys.  Zeit. 
1905,  6.  339.) 

Solubility  in  H2O  at  t°. 
Coefficient    of   solubility  =  cone,    of    the 
emanation  in  the  liquid:  cone,  of  the  emana- 
tion in  the  gas. 


t 

Coefficient  of  solubility 

0 

0.506 

4.3 

0.424    . 

5.7 

0.398 

10.0 

0.340 

14.0 

0.303 

17.6 

0.280 

20.0 

0.245 

26.8 

0.206 

31.6 

0.193 

39.1 

0.160 

Coefficient    of  solubility  in  sea-water    of 
sp.  gr.  at  14°  =  1.022  is  0.255. 

(Boyle,  Phil.  Mag.  1911,  (6)  22.  850.) 


772 


RHODICYANHYDRIC  ACID 


Solubility  in  H2O. 
Temp.        0.5°      17.5° 
Sol.  0.526     0.283 


35° 
0.183 


41° 
0.161 


Temp. 
Sol. 


60°  74°  79°  82° 
0.127  0.112  0.111  0.111 
(Kofler,  M.  1913,  34.  389.) 


51° 
0.138 

91° 
0.108 


Coefficient  of  solubility  of  radium  emana- 
tion at  14°  in  various  solvents. 


Ethyl  alcohol 
Amyl  alcohol 
Toluene 
Sea  water 
Mercury 


7.34 
9.31 
13.7 
0,255 
0 


(Boyle,  Phil.  Mag.  1911,  (6)  22.  851.) 


Coefficient  of  solubility  emanation  of  radium 
in  various  solvents  at  t°. 


Solvents 

t=18° 

t=o° 

t  = 

—18° 

Ethyl  acetate 

7.35 

9.41 

13.6 

Acetone 

6.30 

7.99 

10.8 

Absolute 

alcohol 

6.17 

8.28 

11.4 

Aniline 

3.80 

4.43 

Benzene 

12.82 

16.54  at  3° 

Chloroform 

15.08 

20.5 

28^5 

Cylclohexane 

18.  04  at  80° 

Water 

0.285 

6!52 

Ether 

15.08 

20.09 

29!  i 

Glycerine 

0.21 

Hexane 

16.56 

23^4 

35^2 

Paraffine  oil 

9.2 

12.6 

Carbon- 

bisulphide 

23.14 

33.4 

50.3 

Toluene 

13.24 

18.4 

27 

Xylene 

12.75 

(Ramstedt,  Le  Radium,  1911,  8.  255.) 


Solubility  in  various  oils,  etc.,  at  t°. 


Rape  oil 

Poppy  seed  oil 

Oil  of  turpentine 

t° 

-3 

10 
20 
100 

200 

Solubility 

51.2 
35.3 
26.1 
6.2 
3.3 

t° 

Solubility 

t° 

Solubility 

-5 
16 
40 
65 
90 

50.5 
30.2 
19.1 
12.4 

8.4 

-21 

0 
18 
50 
6.5 

42.5 
23.1 
16.6 
7.5 
4.08 

Solubility  in  10%  dammar  resin  in  oil  of 
turpentine  =  16 . 7  at  18°. 

Solubility    in     5%    colophony     in    amyl 
alcohol  =  11. 2  at  20C. 

Solubility  in  amyl  alcohol  =  10.6  at  18°. 

Solubility    in    20%     colophony    in    amyl 
alcohol  =  11.1  at  20°. 

(Curie,  Thesis.  1910.) 


Coefficient  of  absorption  for  petroleum  = 
22.70  at  -21°. 
12.87  at  +3°. 
9.55  at  20°. 
8.13  at  40°. 
7.01  at  60°. 
(Hofmann,  Phys.  Zeit.  1905,  6.  339.) 

Rhodicyanhydric  acid,  H3Rh(CN)6. 
Not  known  in  the  free  state. 

Potassium  rhodicyanide,  K3Rh(CN)6. 
Sol.  in  H2O.    Easily  decomp.  by  acids. 
Very  sol.  in  H2O.    (Leidi<§,  C.  R.  1900,  130. 

89.) 

Rhodium,  Rh. 

Insol.  in  all  acids,  including  aqua  regia. 
Rhodium  "sponge"  is  sol.  in  HNO3+Aq, 
and  somewhat  in  HCl+Aq  when  exposed  to 


Rhodium  ammonia  compounds. 

See— 

Bromopurpureorhodium  comps., 
BrRh(NH3)6X2. 

Chloropurpureorhodium  comps., 
ClRh(NH3)5X2. 

lodopurpureorhodium  comps., 
ERh(NH.)«X* 

Luteorhodium  comps.,  Rh(NH3)6X3. 

Nitratopurpureorhodium  comps., 
(NO3)Rh(NH3)5X2. 

Roseoihodium  comps.,  Rh(NH3)5(OH2)X3. 

Xanthorhodium  comps.,  ^  NO2)Rh(NH3)5X2. 

Rhodium  ^bromide,  RhBr3+2H20. 

Very  sol.  in  H2O.  (Goloubkine,  Chem. 
Soc.  1911,  100.  (2)  45.) 

Rhodium  rubidium  bromide. 
See  Bromorhodite,  rubidium. 

Rhodium  sodium  bromide. 
See  Bromorhodite,  sodium. 

Rhodium  ^chloride,  RhCl2  (?). 

Insol.  in  H2O,  HC1,  or  HNO3+Aq.     Not 

attacked  by  boiling  KOH   or  K2CO3+Aq. 

(Fellenberg.) 

Decomp. by  boiling  KOH + Aq.  (Berzelius.) 
Does  not  exist.    (Leidie",  C.  R.  106.  1076. 

Rhodium  ^n'chloride,  RhCl3. 

Insol.  in  acids,  even  aqua  regia.  When 
boiled  for  a  long  time  with  KOH+Aq,  it  be- 
comes si.  sol.  in  HCl+Aq. 

Insol.  in  H2O  and  acids;  sol.  in  alkalies+Aq. 
(Leidie*,  C.  R.  18P9,  129.  1251.) 

+4H2O.  Very  si.  deliquescent.  Easily  sol. 
in  H2O,  HCl+Aq,  or  alcohol.  Insol.  in  ether. 
Decomp.  by  H2SO4  only  when  boiling.  (Glaus, 
J.  pr.  80.  282.) 


RHOlfoCHROMIUM  SULPHATE 


773 


No  definite  amount  of  crystal  H2O.  (Leidie" 
A.  ch.  (6)  17.  271.) 

Rhodium  chloride  with  MCI.. 
See  Cblororhodite,  M. 

Rhodium     dzhydroxide,     RhO2,     2H2O,     or 
Rhodium  rhodate,  Rh2O3,  RhO3+6H2O. 
Sol.  in  HCl+Aq. 

Rhodium  sesgiuhydroxide,  Rh2O6H6. 

Only  si.  sol.  in  cone.  HCl+Aq.  (Glaus.) 
+2H2O.  Easily  sol.  in  HC1,  H2SO4,  H2SO3, 
HNO3,  or  HSCN+Aq;  also  when  moist,  in 
HC2H3O2 + Aq.  Sol.  in  cone.  KOH  +  Aq ;  very 
si.  sol.  in  H3BO3,  H3PO4,  H2C4H4O6,  and  HCN 
+Aq.  Sol.  in  acid  alkali  oxalates+Aq. 
(Leidie",  C.  R.  107.  234.) 

Rhodium  Zniodide,  RhI3. 

Ppt.     (Goloubkine,  Chem.  Soc.  1911,  100. 

(2)  45.) 

Rhodium  monoxide,  RhO. 

Not  attacked  by  acids.  (Deville  and  De- 
bray,  A.  ch.  (3)  61.  83.) 

Rhodium  ses^wioxide,  Rh2Os. 

Insol.  in  H2O,  boiling  KOH+Aq,  or  any 
acid,  even  aqua  regia.  (Glaus.) 

Rhodium  dioxide,  RhO2. 

Insol.  in  all  acids  or  alkalies. 

Rhodium  ^noxide,  RhO3. 

"Rhodic  acid."  Known  only  in  solution  of 
" Potassium  rhodate,"  which  is  very  easily 
decomp.  (Glaus.) 

Rhodium  oxybromide,  Rh(OH)2Br+2H2O. 

Sol.  in  H2O.  (Goloubkine,  Chem.  Soc. 
1911,  100.  (2)  45.) 

Rhodium  raonosulphide,  RhS. 
Insol.  in  aqua  regia.     • 

Rhodium  sesgiwsulphide,  Rh2S3. 

Sol.  in  alkali  sulphides +Aq.  (Debray,  C. 
R.  97.  1332.) 

Insol.  in  alkali  sulphides +Aq.  Not  at- 
tacked by  HNO3,  aqua  regia,  or  Br2+Aq. 
(Leidie,  Bull.  Soc.  (2)  50.  664.) 

Rhodium  sodium  sulphide,  3Na2S,  Rh2S3. 
Decomp.  by  H2O.    (Leidie".) 

Rhodium  sesgiusulphydroxide,  Rh2S6H6. 

Easily  sol.  in  aqua  regia  or  Br2  +Aq.  Insol. 
in  alkali  sulphides +Aq  or  acids.  (Leidie", 
Bull.  Soc.  (2)  60.  664.) 


Rhodochromium  bromide, 

HOCr2(NH3)10Br5+H2O. 
Rather  difficultly  sol.  in  H2O.  Decomp.  by 
boiling  or  standing.  Sol.  in  NH4OH+Aq 
or  NaOH+Aq.  Insol.  in  dil.  HBr+Aq, 
KBr+Aq,  or  alcohol.  (Jorgensen,  J.  pr.  (2) 
26.321.) 


—  bromide,  basic,  HOCr2(NH3)10(OH)Br4 

+H20. 

SI.  sol.  in  H2O.    Sol.  in  NH4OH  or  NaOH  + 
Aq.    Insol.  in  alcohol.    (Jorgensen.) 


—  bromoplatinate,  HOCr2(NH3)10Br3PtBr6, 

HOCr2(NH3)10Br3(PtBr6)2+4H2O. 
Ppt.    (Jorgensen.) 

chloraurate,  HOCr2(NH3)10Cl3(AuCl4)2 

+2H2O. 

Difficultly  sol.  but  not  insol.  in  H2O.  (Jor- 
gensen). 

chloride,  HOCr2(NH3)ioCl6+H2O. 

Sol.  in  about  40  pts.  of  cold  H2O.  Insol.  in 
cold  dil.  HCl+Aq,  NH4Cl+Aq,  or  alcohol. 
Sol.  in  NH4OH+Aa.  C  Jorgensen,  J.  pr.  (2) 
25.  321.) 

— —  chloroiodide,  basic, 

HOCr2(NH3)  10(OH)C12I2. 
SI.    sol.   in   cold   H2O;   insol.   in   alcohol. 
(Jorgensen.) 

•  chloroplatinate,  HOCr2(NH3)ioCl3PtCl6, 

HOCr2(NH?)10Cl(PtCl6)2+4H2O. 
Precipitate.    (Jorgensen.) 

dithionate,     [HOCro(NH3)10]2(S2O6)5  + 

2H2O. 

Nearly  insol.  in  H2O.  * 


— —  dithionate,  basic, 

HOCr2(NH3)10OH(S2O6)2+H2O. 
Insol.    in    H2O,    cold    NH4OH+Aq,    or 
NaOH+Aq. 

—  iodide,  HOCr2(NH3)10I8+H2O. 

Very  difficultly  sol.  in  H2O.  Insol.  in  very 
dil.  HI+Aq  or  alcohol.  SI.  sol.  in  NH4OH  or 
KOH+Aq.  (Jorgensen.) 

-  nitrate,  HOCr2(NH3):o(NO3)&. 

Rather  difficultly  sol.  in  H2O,  from  which 
it  is  precipitated  by  a  few  drops  of  HNO3+ 
Aq.  Sol.  in  hot  dil.  NH4OH+Aq. 

— —  nitrate  chloroplatinate, 

HOCr2(M  H8)  io(NO3)  (PtCl6)2 +4H2O. 
Precipitate.    (Jorgensen.) 

Rhodochromium  sulphate, 

[HOCr2(NH3)10]2(SO4)5+2H2O. 
Very  si.  sol.  in  cold  H2O.     Easily  sol.  in 
cold  dil.  H2SO4+Aq. 


774 


RHODONITROUS  ACID 


Almost  insol.  in  a  mixture  of  3  vols.  H2O, 
1  vol.  alcohol,  and  l/3  vol.  dil.  H2SO4+Aq. 
(Jorgensen.) 

Rhodonitrous  acid. 

Ammonium  rhodonittite,  (NH4)6Rh2(NO2)i2. 

Nearly  insol.  in  cold,  si.  sol.  in  hot  H2O. 
Insol.  in  cone.  JNH4C1  or  NH4C2H3O2+Aq. 
Insol.  in  alcohol.  (Leidie",  C.  R.  111.  108.) 

Barium  rhodonitrite,  Ba3Rh2(NO2)i2. 

SI.  sol.  in  cold,  more  easily  in  hot  H2O. 
(Lamy.) 

+  12H2O.  Sol.  in  50  pts.  H2O  at  16°,  and 
6.5  pts.  at  100°.  (Leidie*,  C.  R.  111.  108.) 

Potassium  rhodonitrite,  K6Rh2(NO2)]2. 

Nearly  insol.  in  cold,  very  si.  sol.  in  boiling 
H2O.  Completely  insol.  in  KNO2+Aq,  and 
in  KCl+Aq  (30%  KC1),  or  KC2H3O2+Aq 
(50%KC2H3O2).  Insol.  in  alcohol.  (Leidie*, 
C.  R.  111.  106.) 

Sodium  rhodonitrite,  Na6Rh2(NO2)12. 

Sol.  in  2^2  pts.  H2O  at  17°,  and  1  pt.  at 
100°.  Insol.  in  alcohol.  Decomp.  by  HC1+ 
Aq.  (Leidie",  C.  R,  111.  107.) 

Rhodosochromium  bromide. 

Sol.  in  H2O;  insol.  in  dil.  HBr+Aq  (I  :  1). 
(Jorgensen,  J.  pr.  (2)  46.  260.) 

chloraurate,  Cr2(NH3)6(HO)3Cl3, 

2AuCl3+2H2O. 
Not  insol.  in  cold  H2O.    (Jorgensen.) 

—  chloride,  Cr2(NH3)6(HO)3Cl3+2H2O. 

Sol.  in  10.6  pts.  H2O  at  18°;  decomp.  by 
boiling.  Pptd.  by  ^  to  1  vol.  dil.  HCl+Aq. 
Sol.  in  cold  dil.  NH4OH+Aq.  (Jorgensen,  J. 
pr.  (2)  46.  260.) 


chloroplatinate,  2Cr2(NH3)6(OH)3Cl3, 

3PtCl4+6H2O. 

Insol.  in  H2O.    (Jorgensen.) 

Cr2(NH3)6(OH)3Cl3, 2PtCl4+2H2O.     Insol. 
in  95%  alcohol.    (Jorgensen.) 

chromate,  [Cr2(NH3)6(OH)3]2(CrO4)3  + 

7H2O.    (Jorgensen.) 
Very  si.  sol.  in  H2O.    (Jorgensen.) 

iodide,  Cr2(NH3)6(OH)3I3+2H2O. 

Sol.  in  H2O.    Insol.  in  dil.  HI+Aq.    (Jor- 
gensen.) 

nitrate,  Cr2(NH3)6(OH)3(NO3)3+H2O. 

Much  less  sol.  in  cold  H2O  than  the  chloride. 
Insol.  in  dil.  HNO3+Aq.    (Jorgensen.) 

oxalate, 

[Cr2(NH3)6(OH)3]2(C204)(HC204)4  + 
2H2O. 

Sol.  in  cold  H2O,  but  not  very  easily.    (Jor- 
gensen.) 


Rhodosochromium  sulphate, 

[Cr2(NH3)6(OH)3]2(SO4)3+5H2O. 

Very  si.  sol.  in  cold  H2O.  Easily  sol.  in  dil. 
NH4Cl+Aq.  (Jorgensen.) 

[Cr2(NH3)6(OH)3]SCL,  HSO4+1^H2O.  De- 
comp. by  H2O  into  H2SO4  and  above  com- 
pound. (Jorgensen.) 

ulphide,  [Cr2(NH3)6(OH)3]2Sn  + 


Ppt.    Insol.  in  H2O.    (Jorgensen.) 
Rhodosulphuric  acid. 

Potassium  rhodosulphate,  K6Rh2(SO4)6. 
Two  modifications: 

(a)  Slowly  sol.  in  cold,  easily  in  hot  H2O. 

(b)  Insol.  in  H2O. 

Does  not  exist.    (Leidie*,  C.  R.  107.  234.) 

Sodium  rhodosulphate. 

Insol.  in  H2O,  HC1,  HNO3,  or  aqua  regia. 
(Claus.) 

Does  not  exist.    (Leidie".) 

Na2Rh2(SO4)4.  Insol.  in  H2O.  (Seubert 
and  Kobbe*,  B.  23.  2560.) 

Rhodosulphurous  acid. 

Potassium  rhodosulphite,  KeRh2(SO3)5  + 

6H20. 

Nearly  insol.  in  H2O.  Slowly  sol.  in  acids. 
Not  decomp.  by  boiling  KOH+Aq.  (Claus.) 

Sodium  rhodosulphite, 

Na6Rh2(SO3)5+4^H2O  =  3Na2SO3, 
2RhSO3. 

Insol.  in  cold,  very  si.  sol.  in  hot  H2O. 
Easily  sol.  in  HNO3+Aq.  (Seubert  and 
Kobbe",  B.  23.  2558.) 

Roseochromium  bromide, 

Cr(NH3)5Br3+H20. 

Easily  sol.  in  H2O.  Insol.  in  HBr+Aq. 
(Christensen,  J.  pr.  (2)  23.  26.) 

—  bromochromate,  Cr(NH3)5Br(CrO4). 
Somewhat  sol.  in  H2O,  but  decomp.   on 

standing.    (Jorgensen,  J.  pr.  (2)  25.  398.) 

—  bromoplatinate,    Cr(NH3)5Br(PtBr6)  + 
2H2O. 

Precipitate.  Difficultly  sol.  in  H20.  (Chris- 
tensen, I.  c.) 

—  chloride,  Cr(NH3)5Cl3+H20. 

Easily  sol.  in  H2O  with  subsequent  decomp. 
Insol.  in  alcohol.  (Christensen,  J.  pr.  (2)  23. 

26.) 

mercuric  chloride,  Cr(NH3)5Cl3,  3HgCU 

+2H2O. 

SI.  sol.  in  H2O.  Sol.  in  dil.  HCl+Aq  with 
decomposition.  (Christensen,  I.  c.} 


ROSEOCOBALTIC  MERCURIODIDE 


775 


Roseochromium  dithionate,  basic, 

Cr(NH3)6(OH)2S2O6+H2O. 
Easily  sol.  in  very  dil.  HCl+Aq.    (Jorgen- 
sen,  J.  pr.  (2)  25.  398.) 

—  iodide,  Cr(NH3)5l3. 
Easily  sol.  in  H2O;  decomp.  by  boiling. 
(Christensen,  I.  c.) 

nitrate,  Cr(NH3)6(NO3)3+H2O. 

Rather  easily  sol.  in  H2O.  (Christensen, 
I.  c.) 

Cr(NH3)5(NO3)3(OH2)2,  HNO3.  Decomp. 
by  H2O  or  alcohol.  (Jorgensen,  J.  pr.  (2)  44. 

—  sulphate,  [Cr(NH3)5]2(SO4)3+5H2O. 

Easily  sol.  in  H2O.  Precipitated  by  alcohol. 
(Christensen,  I.  c.) 

— —  sulphate  bromoplatinate, 

[Cr(NH3)5(S04)]2PtBr6. 
Difficultly  sol,  in  H2O.    (Christensen,  I.  c.) 

— — •  sulphate  chloroplatinate, 

[Cr(NH3)5(S04)j2PtCl6. 
Difficultly  sol.  in  H2O.    (Christensen,  I.  c.) 

Roseocobaltic  bromide, 

Co(NH3)5(OH2)Br3. 

Sol.  in  H2O;  insol.  in  HBr+Aq.  (Jorgen- 
sen, J.  pr.  (2)  31.  49.)  3 

— —  bromoplatinate,  Co(NH3)6(OH2)Br3, 
PtBr4+H2O. 

Somewhat  sol.  in  H2O  or  dil.  alcohol.  Insol 
in  strong  alcohol.  (Jorgensen.) 

2Co(NH3)5(OH2)Br3,  3PtBr4+4H2O.  Ppt. 
(Jorgensen.) 

bromosulphate, 

Co(NH3)5(OH2)Br(SO4). 
Sol.  inH2O.    (Krok.) 

bromosulphate  bromaurate, 

Co(NH3)5(OH2)(S04)Br,  AuBr3. 

carbonate. 

Very  sol.  in  H2O. 

chloraurate,  Co(NH3)6(OH2)Cl3,  AuCl3. 

Moderately  sol.  in  cold  H2O. 

—  chloride,  Co(NH3)5(OH2)Cl3. 

Sol.  in  4.8  pts.  H2O  at  10.1°,  but  decomp. 
on  heating. 

100  pts.  H2O  dissolve  16.12  pts.  at  0°,  and 
24.87  pts.  at  16.19°.  (Kurnakoff,  J.  russ  Soc 
24.  269.) 

SI.  sol.  in  1000  pts.  fuming  HCl+Aq,  more 
easily  in  20%  HCl+Aq.  (Rose.) 


Roseocobaltic  mercuric  chloride, 

Co(NH8)6(OH2)Cl3,  3HgCl2+H2O. 

More    easily    sol.    in    solvents    than    the 
anhydrous  purpureo  salt.    (Carstanien.) 

Co(NH3)5(OH2)Cl3,  HgCl2.    Sol.  in  HC1+ 
Aq  with  decomp.  into  above  salt.  (Jorgensen.) 


chloroplatinate, 


Co(NH3)5(OH2)Cl3,  PtCl4+^H20. 

Decomp.  by  H2O.    (Jorgensen.) 

2Co(NH»)«(OHi)Cl,,  PtCl4+2H20.  De- 
comp. by  H2O. 

2Co(NH3)5(OH2)Cl3,  3PtCl4+6H2O.  Not 
difficultly  sol.  in  warm  H2O.  (Gibbs.) 

Co(NH3)5Cl3,  PtCl4+H2O.    (Gibbs.) 

—  chlorosulphate,  Co(NH3)5Cl(SO4). 
Easily  sol.  in  H2O. 

•  chlorosulphate  mercuric  chloride, 

Co(NH3)5Cl(SO4),  HgCl2+3H2O. 
Sol.  in  hot  H2O,  and  can  be  recrystallized 
without  decomp.    (Krok.) 

cfa'chromate, 

[Co(NH3)5]2(Cr207)3+5H20. 
Can  be  recrystallized  out  of  weak  acetic 
acid. 

cobalticyanide,Co(NH3)6(OH2)Co(CN)6. 

Nearly  absolutely  insol.  in  cold  H2O.  (Jor- 
gensen.) 

+H2O.    (Gibbs  and  Gentele.) 

—  dithionate,  Co(NH3)5(S2O6)(OH). 

Decomp.  by  H2O.  (Rammelsberg,  Pogg. 
58.  296.) 

Co(NH3)5(OH2XS206)+2H20.  Ppt.  (Jdr- 
gensen.) 

—  hydroxide,  Co(NH2)5(OH)3. 
Known  only  in  aqueous  solution. 

- —  mercuric  hydroxychloride, 
CoN5H12(HgOH)3Cl3. 

Ppt.  Sol.  in  dil.  acids.  (Vortmann  and 
Morgulis,  B.  22.  2646.) 

CoN6H12(HgOH)3Cl2(OH).  Ppt.  Sol.  in 
dil.  acids.  (Vortmann  and  Morgulis.) 

—  iodide,  Co(NH3)5(OH2)I3. 

Less  sol.  in  H2O  than  bromide.  Insol.  in 
HI+Aq.  (Jorgensen.) 

—  iodosulphate,  Co(NH3)6(OH2)I(SO4). 
Easily  sol.  in  H2O.    (Krok.) 


—  meicuriodide,  [CoN5Hi3]2(HgI)3I6. 

Ppt.  (Vortmann  and  Borsbach,  B.  23. 
2805.) 

CoN6H13(HgI)  2I3.  Ppt.  (Vortmann  and 
Borsbach.) 

CoN6H13(HgI)2I2(OH).    Ppt. 


776 


ROSEOCOBALTIC  NITRATE 


Roseocobaltic  nitrate, 

Co(NH3)5(OH2)(N03)3. 

Three  modifications: 

a.  Sol.  in  20  pts.  H2O  at  15°.     (Jorgensen.) 

/3.  Known  only  in  solution.  Insol.  in  cold 
HNO3+Aq.  (Gibbs.) 

7.  Easily  sol.  in  hot  H2O.  (Gibbs.)  (Pur- 
pureo  salt  ?) 

Co(NH?)5(OH2)(NO3)3,  HNO3.  Decomp. 
by  H2O  or  alcohol.  (Jorgensen,  J.  pr.  (2)  44. 
63.) 

nitrate  chloroplatinate, 

Co(NH3)6(OH2)(NO3)Cl2,  PtCl4+H2O. 
Ppt.    (Jorgensen.) 

niti  atosulphate, 

Co(NH3)5(OH2)(N03)(S04). 
SI.  sol.  in  cold,  easily  in  hot  H2O. 

oxalate,   [Co(NH3)5(OH2)]2(C2O4)3  + 

2H2O. 

Nearly  insol.  in  H2O. 
[Co(NH3)6]2(C204)3,  4H2C204. 

•  oxalochloroplatinate, 

[Co(NH3)5J2C204Cl2,  PtCl4. 
Sol.  in  hot  H2O. 


oxalosulphate,  [Co(NH3)6]2(SO4)2C2O4, 

H2C204+2H20. 

Sol.  in  hot  H2O. 

[Co(NH3)6]2(SO4)2(C2O4)(OH)2+6H2O.  SI. 
sol.  in  H2O. 


orthophosphate, 

Co(NH3)5(OH2)(PO4H)(OH)+xH2O. 

Nearly  insol.  in  H2O. 

[Co(NH3)5(OH2)]2(Pq4H)3+4H2O.  Very 
si.  sol.  in  cold  H2O;  easily  in  H2O  containing 
HC1.  (Jorgensen.) 

•  p?/rophosphate, 

[Co(NH3)  6(OH,)]  4(P207)  3 .+  12H20. 

Insol.  in  H2O.    (Jorgensen.) 

Co(NH3)6(OH2)(P2O7]Na)  +  12H2O.  Nearly 
insol.  in  cold,  easily  sol.  in  hot  H2O  containing 
NH4OH.  (Jorgensen,  J.  pr.  (2)  23.  252.) 

sulphate,   [Co(NH3)5(OH2)]2(SO4)3+ 

3H2O. 

Three  modifications: 

a.  SI.  sol.  in  cold  H2O.  Sol.  in  58  pts.  at 
27°  (Gibbs);  83.5  pts.  at  20.2°,  and  94.6  pts 
at  17.2°  (Jorgensen);  more  easily  sol.  in  hot 
H2O,  and  still  more  easily  in  NH4OH+Aq. 

/3.  Sol.  in  1-2  pts.  H2O.    (Gibbs.) 

7.  Less  sol.  than  luteosulphate.  (Jorgen- 
sen.) 

+2H2O.    Easily  sol.  in  H2O.    (Vortmann.) 


Roseocobaltic  sulphate,  acid, 

[Co(NH3}6]2(SO4)r,    2H2SO4+3H2O. 

(Fremy),  or  4[CoCNH»)«}»(SO,},,  9H2SO4 

+  11H2O  (Jorgensen). 

More  easily  sol.  in  H2O  than  neutral  sul- 
phate, into  which  it  is  converted  by  recrystal- 
lization.  Sol.  in  about  13  pts.  H2O.  (Jorgen- 
sen.) 


cerium  sulphate, 

[Co(NH3)5(OH2)]2(S04)3,    Ce2(S04)3  + 


SI.  sol.  in  cold,  practically  insol.  in  boiling 
H2O.  Sol.  in  acids.  (Gibbs,  Am.  Ch.  J.  15! 
560.) 

[Co(NH3)5(OH2)]2(S04)3,  Ce(S04)2  + 
.    As  above.    (Gibbs.) 


sulphate  chlorauiate. 


Ppt. 


Three  modifications: 

a.  Co(NH3)5(OH2)(SO4)Cl,    AuCl3. 
( Jorgensen.) 

/3.  CWNH,)6(SOi);  AuCl3+2H2O.     SI.  sol. 
in  cold  H2O.    (Gibbs.) 

7.  As  above.     Can  be  recrystallized  from 
hot  H2O. 

— —  sulphate  chloioplatinate, 

2Co(NH3)6(OH2)(SO4)Cl2,  PtCl4. 
Three  modifications,  all  difficultly  sol.  in  hot 
or  cold  H2O.    CJorgensen.) 

sulphite,  [Co(NH3)6(OH2)J2(SO3)3+H2O. 

SI.    sol.    in   cold,    decomp.    by   hot    H2O. 
(Gibbs.) 

cobaltic  sulphite, 

[Co(NH3)5]2(SO3)3,  Co2(SO3)3+9H2O. 
Insol.  in  cold,  decomp.  by  hot  H2O.   (Kiin- 
zel.) 

Roseocobaltic  octamine  compounds. 
See  Roseotetramine  cobaltic  compounds. 

Roseoiridium  compounds. 

See  Iridoaquopentamine  compounds. 

Roseorhodium  bromide, 

Rh(NH3)5(OH2)Br3. 

Sol.  in  cold  H2O.    (Jorgensen,  J.  pr.  (2)  34. 
394.) 

Roseorhodium  cobalticyanide, 

Rh(NH3)5(OH2)Co(CN)6. 
Scarcely  sol.  in  H2O. 

—  iodosulphate,  Rh(NH3)6(OH2)I(SO4). 
Very  si.  sol.  in  H2O;  easily  sol.  in  NH4OH  + 

Aq.    (Jorgensen.) 

—  nitrate,  Rh(NH3)5(OH2)(NO3)3. 
Moderately  sol.  in  cold  H2O.    (Jorgensen.) 
Rh(NH3)6(OH2)(NO3)3,  HNO3.     Decomp. 


RUBIDIUM   BROMIDE 


777 


by  H2O  or  alcohol.    (Jorgensen,  J.  pr.  (2)  44. 
63.) 

Roseorhodium  nitrate  chloroplatinate, 

[Rhf  NH3)  5(  OH2)  (NO,)]  2PtCl6 +2H2O . 
Ppt.    (Jorgensen.) 

or/ftophosphate, 

[Rh(NH3)6(OH2)]2(HP04)3+4H20. 
Very  si.  sol.  in  H2O. 

sodium  p7/rophosphate, 

[Rh(NH3)5(OH2)]2NaP2O7+23H2O. 
Ppt.    Very  si.  sol.  in  cold  H2O.    Easily  sol. 
in  very  dil.  acids. 

sulphate, 

•      lRh(NH3)5(OH2)2](SO4)3+3H2O. 
Very  si.  sol.  in  cold,  much  more  in  hot  H2O. 

sulphate  chloroplatinate, 

Rh(NH3)5(OH2)(SO4)PtCl6. 
Ppt.    Nearly  insol.  in  H2O  or  alcohol. 

Roseotetramine  cobaltic  bromide, 

Co(NH3)4(OH2)2Br3. 

Sol.  in  H2O;  insol.  in  HBr+Aq.    Nearly  in- 
sol. in  alcohol.    (Jorgensen,  Z.  anorg.  2.  295.) 

—  chloride,  Co(NH3)4(OH2)2Cl3. 
Easily  sol.  in  H2O;  insol.  in  cone.  HCl+Aq; 
sol.  in  sat.  HgCl2+Aq.    (Jorgensen.) 

—  cobalticyanide, 

Co(NH3)4(OH2)2Co(CN)6. 
(Jorgensen.) 


oxalate  sulphate, 


[Co(NH3)4(OH2)2MS04)2C204. 
Ppt.    (  Jorgensen.) 


--  —  p2/rop 

[Co(NH3)  4(OH2)  J  4(P207)  ,  +6H20. 
Nearly  insol.  in  H2O,  but  easily  sol.  in  very 
dil.  acids  +Aq.    (Jorgensen.) 

---  sulphate, 

[Co(NH3)4(OH2)2]2(S04)3+3H20. 
Sol.  in  about  35  pts.  H2O,  and  more  easily 
by  addition  of  dil.  HC1  or  H2SO4+Aq.    (Jor- 
gensen.) 

---  sulphate  bromaurate. 

[Co(NH3)4(OH2)2]2(S04)2AuBr4. 
SI.    sol.    in    cold   H2O;   insol.    in   alcohol. 
(Jorgensen.) 


sulphate  chloroplatinate, 

[Co(NH3)4(OH2)2]2(SO4)2PtCl6. 
As  the  bromaurate.    (Jorgensen.) 


Rubidium,  Rb2. 

Decomp.  H2O  with  violence.  Insol.  in 
hydrocarbons.  Sol.  in  liquid  NH3.  (Seely, 
C.  N.  23.  169);  (Franklin,  Am.  Ch.  J.  1898, 
20.  829). 

Rubidium  acetylide  acetylene  RbC2,  C2H2. 

Very  hygroscopic. 

Insol.  in  CC14  and  in  ether.  (Moissan,  C. 
R.  1903,  136.  1220.) 

Rubidium  amalgam,  RbHgi2. 

Stable    in    contact    with    Hg    below    0°. 

Above  0°  the  composition  of  the  amalgam 
varies.  Can  be  cryst.  from  Hg  without  de- 
comp.  below  0°.  (Kerp,  Z.  anorg.  1900,  26. 
68.) 

Rubidium  amide,  RbNH2. 

Very  deliquescent.  Violently  decomp.  by 
H2O;  less  violently  acted  on  by  alcohol. 
(Titherley,  Chem.  Soc.  1897,  71.  470.) 

Rubidium  ammonia,  RbNH3. 

Decomp.  by  H2O. 

Very  sol.  in  liquid  NH3.  (Moissan,  C.  R. 
1903,  136.  1178.) 

Rubidium    azoimide,    RbN3. 

SI.    hydroscopic. 

Stable  in  aq.  solution. 
107. 1  pts.  are  sol.  in  100  pts.  H2O  at  16°. 
114.1     "      "     "     "  100     "    H2O  "   17°. 
0.182     "      "     "     "100     "    abs.  alcohol  at 
16°. 

Insol.  in  pure  ether. 

(Curtius,  J.  pr.  1898,  (2)  68.  281.) 

Rubidium  bromide,  RbBr. 

100  pts.  H2O  dissolve  98  pts.  at  5°;  104.8* 
pts.  at  16°.  (Reissig,  A.  127.  33.) 

Solubility  in  H2O. 

100  pts.  of  the  solution  contain  at: 
0.5°  5.0°  16.0° 

47.26          49.50  51 . 17  pts.  RbBr, 

39.7°  57.5°  113.5° 

56 .87          60 . 39  67 . 24  pts.  RbBr. 

(Rimbach,  B.  1905,  38.  1557.) 

Sp.  gr.  of  RbBr  containing  g.  equiv.  RbBr 
per  1. 


G.  equiv. 
RbBr 

Sp.gr. 

6°/6° 

Sp.  gr. 

18°,'  18° 

Sp.  gr. 
30°/30° 

0.508 

1.020 
2.031 

4.072 

1.06448 
1.12931 
1.25622 
1.50574 

1.06389 
1.12799 
1.25366 
1.50107 

1.06326 
1.12626 
1.25187 
1.49870 

(Clausen,  W.  Ann.  1914,  (4)  44.  1070.) 


778 


RUBIDIUM   BROMIDE 


RbBr+Aq.  containing  6.60%  RbBr  has 
sp.gr.  20°/20°  =  1.0525. 

RbBr+Aq.  containing  14.36%  RbBr  has 
sp.  gr.  20°/20°  =  1.1226. 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  279.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014.) 

Difficultly   sol.    in    acetone.      (Naumann, 

B.  1904,  37.  4328.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,42.3790.) 

Rubidium  ^n'bromide,  RbBr3. 

Very  sol.  in  H2O;  decomp.  by  alcohol 
and  ether.  (Wells  and  Wheeler,  Sill.  Am.  J. 
143.  475.) 

Rubidium  ruthenium  bromide. 

See  Bromoiuthenate  and  bromoruthenite, 
rubidium. 

Rubidium  seleDium  bromide. 
See  Bromoselenate,  rubidium. 

Rubidium  tellurium  bromide. 
See  Biomotellurate,  rubidium. 

Rubidium  thallic  bromide,  RbBr,  TlBr3+H2O. 

Recryst.  from  H2O  unchanged.  (Pratt, 
Am.  J.  Sci.  1895,  (3)  49.  403.) 

3RbBr,  TlBr,+H2O.  Very  sol.  in  H2O. 
(Pratt.) 

Rubidium  stannic  bromide. 
See  Bromostannate,  rubidium . 

Rubidium  bromochloiide,  RbBr2Cl. 

Easily  decomp.,  even  by  H2O.  (Wells  and 
Wheeler.) 

RbBrCl2.  Sol.  in  H2O;  decomp.  by  alcohol 
and  ether.  (Wells  and  Wheeler.) 

Rubidium  bromochloroiodide,  RbBrClI. 

Sol.  in  H2O  and  alcohol.  Decomp.  by  ether. 
(Wells  and  Wheeler.) 

Rubidium  bromoiodide,  RbBr2I. 

Very  sol.  in  H2O.  Sat.  solution  contains 
about  44%  RbBr2I,  and  sp.  gr.  =  3.84.  (Wells 
and  Wheeler.) 

Rubidium  carbide,  Rb2C2. 

Decomp.    violently    by    H2O.      (Moissan, 

C.  R.  1903,136.  1221.) 

Rubidium  chloride,  RbCl. 

100  pts.  H2O  dissolve  76.38  pts.  at  1°;  82.89 
pts.  at  7°.  (Bunsen.) 


Solubility  in  H2O  at  t°. 
100  pts.  of  the  solution  contain  pts.  RbCl. 

t 

Pts.  RbCl 

0.4 
15.5 
57.3 
114.9 

43.61 
46.56 
53.71 
59.48 

(Rimbach,  B.  1902,  36.  1304.) 
Solubility  of  RbCl  in  H2O  at  t°. 

t° 

G.  RbCl  per  100  g. 

t 

G,  RbCl  per  100  g. 

H26 

Solution 

H20 

Solution 

0 
10 
20 
30 
40 
50 

77.0 
84.4 
91.1 
97.6 
103.5 
109.3 

43.5 
45.8 
47.7 
49.4 
50.9 
52.2 

60 
70 
80 
90 
100 
112.9 

115.5 
121.4 
127.2 
133.1 
138.9 
146.6 

53.6 
54.8 
56.0 
57.1 
58.9 
59.5 

(Berkeley,  Phil.  Trans.  Roy.  Soc.  1904,  203, 
A.  189.) 

Sat.  RbCl+Aq  at  25°  contains  48.57% 
RbCl.  (Foote,  Am.  Ch.  J.  1906,  35.  242.) 

Sp.  gr.  of  RbCl+Aq  containing  in  100  pts. 
H20: 

13 .14        25 . 88      33 . 13  pts.  RbCl. 
1.1066       1.2156       1.2675  sp.gr. 
(Tammann,  W.  Ann.  24.  1885.) 

A  normal  solution  of  RbCl  has  sp.  gr.  at 
25°  =  1.0610.  (Wagner,  Z.  phys.  Ch.  1890, 
5.  39.) 

RbCl+Aq  containing  6.64%  RbCl  has 
sp.  gr.  20°/2C°  =  1.0502. 

RbCl+Aq  containing  10.59%  RbCl  has 
sp  gr  20720°  =  1.0815.  (Xe  Blanc  and  Roh- 
land, Z.  phys.  Ch.  1896,  19.  278.) 

Sp.  gr.  20°/4°  of  a  normal  solution  of  RbCl 
=  1.085405.  (Haigh,  J.  Am.  Chem.  Soc. 
1912,  34.  1151.) 

Sp.  gr.  of  RbCl+Aq  sat.  at  t°. 


t° 

Sp.  gr. 

t 

Sp.  gr. 

0.55 
18.7 
31.5 

44.7 

1.4409 
1.4865 
1.5118 
1.5348 

60.25 
75.15 
89.35 
114* 

1.5558 
1.5746 
1.5905 
1.6148 

*  Boiling  point. 

(Berkeley.) 

Sp.  gr.  of  RbCl  containing  g.  equiv.  RbCl 
perl. 


G.  equiv. 
RbCl 

Sp.  gr. 

6°/6° 

Sp.  gr. 

18°/18° 

Sp.  gr. 
30°/30° 

0.5123 
1.001 
2.073 
3.984 

1.06410 
1.08916 
1.18200 
1.34334 

1.04538 
1.08810 
1.17959 
1.33967 

1.04503 
1.08749 
1.17828 
1.33757 

(Clausen,  W.  Ann.  1914,  (4)  44.  1069J 

RUBIDIUM   URANYL  FLUORIDE 


779 


Very  si.  sol.  in  liquid  NH3.    (Franklin,  Am. 
Ch.  Jf  1898,  20.  829.) 
Solubility  in  alcohols  at  25°. 
100  g.  methyl  alcohol  dissolve  1.41  g. 
100  g.  ethyl  alcohol  dissolve  0.078  g. 
100  g.  propyl  alcohol  dissolve  0.015  g. 
100  g.  isoamyl  alcohol  dissolve  0.0025  g. 
(Turner  and  Bissett,  Chem.  Soc.  1913, 103. 
1909.) 

Insol.  in  anhydrous  pyridine  and  in  97% 
pyridine+Aq.  Very  si.  sol.  in  95%  pyridine 
+Aq;  si.  sol.  in  93%  pvridine+Aq.  (Kah- 
lenberg,  J.  Am.  Chem.  Soc.  1908,  30.  1107.) 
Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);acetone;  (Naumann,  B.  1904, 
37.  4329);  (Eidmann,  C.  C.  1899,  II.  1014). 

Rubidium   ruthenium    ^chloride. 
See  Chlororuthenite,  rubidium. 

Rubidium  ruthenium   tetrachloride. 
See  Chlororuthenate,  rubidium. 

Rubidium  oxyruthenium  chloride, 

Rb2RuO2Cl4. 

Ppt.;  decomp.  by  H2O;  sol.  in  cold  HC1. 
(Howe,  J.  Am.  Chem.  Soc.  1901,  23.  779.) 

Rubidium  tellurium  chloride. 
See  Chlorotellurate,  rubidium. 

Rubidium  thallic  chloride,   2RbCl,   T1C13  + 
H2O. 

Can  be  recryst.  from  H2O  without  change 
(Pratt,  Am.  J.  Sci.  1895,  (3)  49.  399.) 

3RbCl,  T1C18.  Crystallizes  from  HC1  solu- 
tion. (Neumann,  A.  244.  348.) 

+H2O.  Very  sol.  in  cold  H2O.  (Pratt 
Am.  J.  Sci.  1895,  (3)  49.  398.) 

+2H2O.  Efflorescent  in  dry  air.  Sol.  in 
7.5  pts.  H2O  at  18°,  and  1.6  pts.  at  100°. 
(Godeffroy,  Zeitschr.  d.  allgem.  osterr. 
Apothekerv.  1880.  No.  9.) 

Rubidium  stannic  chloride. 
See  Chlorostannate,  rubidium. 

Rubidium    titanium    chloride,   2RbCl,   TiCl3 
Sol.  in  H2O.    (Stabler,  B.  1904,  37.  4408.) 

Rubidium  tungsten  chloride,  Rb3W2Cl9. 

SI.  sol.  in  cold,  more  sol.  in  hot  H2O. 

Sol.  in  very  dil.  NaOH+Aq. 

Nearly  insol.  in  most  organic  solvents. 
(Olsson,  B.  1913,  46.  574.) 

Rubidium  uranous  chloride,  Rb2UCl6. 

As  K  salt.  (Aloy,  Bull.  Soc.  1899,  (3)  21. 
264.) 


Rubidium  uranyl  chloride,  2RbCl,  (UO2)C12 

+2H2O. 

Solubility  in  H2O. 
100  pts.  of  the  solution  contain  at: 
24.8°        80.3° 

57 . 8         65 . 73  pts.  UO2C12,  2RbCl. 
(Rimbach,  B.  1904,  37.  467.) 

Rubidium   vanadium   chloride,    Rb2VCl5 
+H20. 

SI.  sol.  in  H2O  and  alcohol. 

Decomp.  by  H2O  on  standing  so  that  it 
dissolves.  (Stabler,  B.  1904,  37.  4411.) 

Rubidium  zinc  chloride,  2RbCl,  ZnCl2. 

Easily  sol.  in  H2O  and  HCl+Aq.  (Godef- 
froy, B.  8.  9.) 

Rubidium  chloride  selenium  dioxide,  RbCl, 

2SeO2+2H2O. 

Sol.  in  H2O.  (Muthmann,  B.  1893,  26. 
1013.) 

Rubidium  chloroiodide,  RbCl2I. 

Properties  are  similar  to  those  of  RbBrClI. 
(Wells.) 

RbCl^.  Sol.  in  alcohol,  not  attacked  by 
ether.  (Wells  and  Wheeler,  Sill.  Am.  J.  144. 
42.) 

Sol.  in  POC13.  (Walden,  Z.  anorg.  1900, 
25.  212.) 

Nearlv  insol.  in  AsBr3.  (Walden,  Z.  anorg. 
1902,  29.  374.) 

Very  stable;  si.  sol.  in  H2O  at  0°;  only  very 
si.  sol.  in  BCJl.  (Erdmann,  Arch.  Pharm. 
1894,  232.  32.)  (C.  C.  1894,  I.  670.) 

Rubidium  fluoride,  RbF. 

Very  sol.  in  H2O.  (Eggeling,  Z.  anorg. 
1905,  46.  174.) 

100  g.  H2O  dissolve  130.6  g.  RbF  at  18°. 
(de  Forcrand,  C.  R.  1911,  152.  1210.) 

Sol.  in  dil.  HF.  (Pennington,  J.  Am.  Chem. 
Soc.  1896,  18.  57.) 

Insol.  in  liquid  NH3.  (Core,  Am.  Ch.  J. 
1898,  20.  829.) 

Rubidium  hydrogen  fluoride,  RbF,  HF. 

Very  deliquescent. 

Insol.    in    alcohol   and    ether.      (Chabrie*, 
C.  R.  1905,  140.  91.) 

Very  hygroscopic.  Sol.  in  H2O.  (Eggeling, 
Z.  anorg.  1905,  46.  175.) 

RbF,  2HF.  Very  si.  sol.  in  H2O.  (Egge- 
ling, Z.  anorg.  1905,  46.  176.) 

Rubidium  silicon  fluoride. 
See  Fluosilicate,  rubidium. 

Rubidium  tantalum  fluoride. 
See  Fluotantalate,  rubidium. 

Rubidium  uranyl  fluoride,  4RbF,  UO2F2  + 

6H2O. 
(Ditte,  C.  R.  91.  115.) 


780 


RUBIDIUM  HYDRIDE 


Rubidium  hydride,  RbH. 

Decomp.  by  H2O  with  evolution  of  H2. 
(Moissan,  C.  R.  1903,  136.  589.) 

Rubidium  hydroxide,  RbOH. 

Deliquescent,  and  very  sol.  in  H2O.  Sol. 
in  alcohol.  (Bunsen.) 

Sat.  RbOH+Aq  contains  64.17%  RbOH  at 
15°.  (de  Forcrand,  C.  R.  1909,  149.  1344.) 

Rubidium  iodide,  Rbl. 

100  pts.  H2O  dissolve  137.5  pts.  at  6.9°; 
152  pts.  at  17.4.°  (Reissig,  A.  127.  33.) 

Sat.  Rbl+Aq.  at  25°  contains  61.93%  Rbl. 
(Foote  and  Chalker,  Am.  Ch.  J.  1908,  39. 
567.) 

Sp.  gr.  of  Rbl+Aa  containing: 

5%  10%          cold  hot 

sat.  sat. 

Sp.gr.  1.0353       1.0755       1.726       1.9629. 

(Erdmann,  Arch.  Pharm.  1894,  232.  25.) 

Sp.  gr.  of  Rbl+Aq  containing  g.  equiv. 
Rbl  per  I, 


G.  equiv. 
Rbl 

Sp.  gr. 
6°/6° 

Sp.  gr. 

18°/18° 

Sp.  gr. 
30°/30° 

0.510 
1.025 
2.025 
4.015 

1.08347 
1.16751 
1.33012 
1.64781 

1.08268 
1  .  16569 
1.32637 
1.64144 

1.08226 
1  .  16433 
1.32531 
1.63780 

(Clausen,  W.  Ann.  1914,  (4)  44.  1070.) 

Nearly  insol.  in  AsBr3.  (Walden,  Z.  anorg. 
1902,  29.  374.) 

Sol.  in  AsCl3.  (Walden,  Z.  anorg.  1900, 
26.  214);  liquid  SO2.  (Walden,  Z.  anorg. 
1902,  30.  161);  S2C12.  (Walden,  Z.  anorg. 
1900,  25.  217):  SO2C12.  (Walden);  POC13. 
(Walden.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3789.) 

Solubility  in  organic  solvents  at  t°. 

C  =  pts.  by  wt.of  Rbl  in  100  ccm.  of  the  sat. 
solution. 

L  =  no.  of  litres  which  at  the  saturation 
temp,  hold  in  solution  1  mol.  Rbl. 


Solvent 

t° 

C 

L 

Furfurol 

25° 

4.93 

4.31 

Acetonitrile 

25° 

1.350 

15.73 

ii 

0° 

1.478 

14.36 

Propionitrile 

25° 

0.305 

69.61 

" 

0° 

0.274 

77.48 

Nitro  methane 

25° 

0.518 

41.00 

a 

0° 

0.567 

37.44 

Acetone 

25° 

0.674 

31.5 

I 

0° 

0.960 

22.1 

(Walden,  Z.  phys.  Ch.  1906,  55.  718.) 


Rubidium  £raodide,  RbI3. 

Very  sol.  in  H2O.  Sol.  in  about  V«  pt.  H2O 
at  20°;  sol.  in  alcohol.  Decomp.  by  ether. 
(Wells  and  Wheller,  Sill.  Am.  J.  143.  475.) 

Solubility  determinations  show  that  RbI3 
is  the  only  polyiodide  of  rubidium  formed  at 
25°.  Rbl 7  and  RbI9,  mentioned  by  Abegg 
and  Hamburger,  (Z.  anorg.  50,  403)  could  not 
be  obtained.  (Foote  and  Chalker,  Am.  Ch. 
J.  1908,  39.  567.) 

Rubidium  silver  iodide,  2RbI,  Agl. 

Easily  decomp.  by  H2O.  (Wells  and 
Wheeler,  Sill.  Am.  J.  144.  155.) 

Rbl,  AgI  +  V2H2O.  (Marsh,  Chem.  Soc. 
1913,  103.  783.) 

Rbl,  2AgI.    Not  deliquescent. 

Very  sol.  in  acetone.  (Marsh,  Chem.  Soc. 
1913,  103.  783.) 

Rubidium  tellurium  iodide. 
See  lodotellurate,  rubidium. 

Rubidium  thallic  iodide,  Rbl,  T1I3+2H2O. 

Decomp.  by  H2O.  (Pratt,  Am.  J.  Sci. 
1895,  (3)  49.  403.) 

Rubidium  nitride, 

Decomp.  by  heat.  (Franz  Fischer,  B.  1910, 
43.  1468.) 

See  also  Rubidium  azoimide. 

Rubidium  dioxide,  Rb02. 

Decomp.  by  H2O.  (Erdmann,  A.  1897, 
294.  68.) 


Rubidium  sulphide,  Rb2S+4H2O. 

Deliquescent;   very  sol.   in  H2O. 
Z.  anorg.  1906,  48.  299.) 


(Biltz, 


Rubidium  bisulphide,  Rb2S2. 

Anhydrous. 

Sol.  in  H2O. 

Very  hydroscopic.     (Biltz,  Z.  anorg.  1906, 
50.  72.)    " 

+H2O.     From  Rb2S2+Aq. 

Hydroscopic.      (Biltz.) 

Rubidium  bisulphide,  Rb2S3. 

Anhydrous. 

Sol.  in  H2O. 

Hydroscopic.     (Biltz,  Z.  anorg.  1906,  50. 
75.) 

+H2O.    From  Rb2S3+Aq.     (Biltz.) 

Rubidium    tefrasulphide    Rb2S4+2H2O. 

Sol.  in  H2O.     (Biltz,  Z.  anorg.  1906,  48. 
304.) 

Rubidium  pewtosulphide,  Rb2Ss. 

Deliquescent.    Decomp.  by  H2O. 

Very  easily  sol.  in  70%  alcohol. 

Insol.  in  ether,  ethyl  sulphide  or  CHC13. 
(Biltz,  B.  1905,  38.  127.) 


RUTHENIUM   NITROSOOXIDE 


781 


Rubidium  hydrogen  sulphide,  RbHS. 

Deliquescent,  very  sol.  in  H2O.  (Biltz, 
Z.  anorg.  1906,  48.  300.) 

Rubidium  copper  tefrasulpbide,  RbCuS4. 

Decomp.  very  slowly  in  the  air. 

SI.  sol.  in  H2O. 

Very  slowly  decomp.  by  cold  cone.,  more 
rapidly  by  hot  cone.,  and  still  more  rapidly 
by  dil.  HC1,  H2SO4  and  HNO3.  SI.  sol.  in 
alcohol.  (Biltz,  B.  1907,  40.  978.) 

Ruthenic  acid. 

Barium  ruthenate,  BaRuO4+H2O. 

Ppt.    (Debray  and  Joly,  C.  R.  106.  1494.) 

Calcium  ruthenate,  CaRuO4.* 
Ppt. 

Magnesium  ruthenate,  MgRuO4. 
Ppt. 

Potassium  ruthenate,  K2RuO4+H2O. 
Very  sol.  in  H2O. 

Perruthenic  acid. 

Potassium  perruthenate,  KRuO4. 

SI.  sol.  in  HoO.  (Debray  and  Joly,  C.  R. 
106.  1494.) 

Sodium  perruthenate,  NaRuO4+H2O. 
SI.  sol.  in  H2O. 

Ruthenium,  Ru. 

Not  attacked  by  acids,  except  aqua  regia, 
which  dissolves  it  only  very  slightly.  (Glaus, 
Pogg.  65.  218.) 

Ruthenium  ammonium  comps. 
See  Ruthenoefo'amine  comps,  etc. 

Ruthenium  ^n'bromide,  RuBr3. 

Sol.  in  H2O.  Solution  decomposes  slowly 
on  standing,  but  rapidly  on  heating.  (Gut- 
bier,  Z.  anorg.  1905,  46.  178.) 

Ruthenium   ^nbromide,   ammonia, 
2RuBr3,  7NH3. 

Sol.  in  H2O  and  ammonia  with  slight  warm- 
ing. 

Insol.  in  alcohol.  (Gutbier,  Z.  anorg. 
1905,  45.  182.) 

Ruthenium  cfo'chloride,  RuCl2. 

Insol.  in  acids,  even  in  aqua  regia.  SI. 
attacked  by  acids.  Traces  are  dissolved  by 
boiling  with  cone.  KOH+Aq. 

4-#H2O.  Known  only  in  aqueous  solution. 
(Glaus,  A.  59.  238.) 


Ruthenium  ^n'chloride,  RuCl?. 

Deliquescent.  Sol.  in  H2O  and  alcohol,  but 
solution  is  decomp.  by  heating  into  Ru2O3  and 
HC1.  (Glaus.) 

Pure  RuCl3  is  insol.  in  cold  H2O,  mineral, 
or  organic  acids.  Slowly  decomp.  by  boiling 
H2O.  Insol.  in  CC14,  CS2,  CHC13/PC13,  or 
ether.  Slowly  sol.  in  hot  absolute  alcohol, 
but  decomp.  into  Ru(OH)Cl2  by  95%  alco- 
hol. (Joly,  C.  R.  114.  292.) 

Hydroscopic. 

Sol.  in  H2O;  decomp.  at  50°. 

Sol.  in  alcohol.  (Gutbier,  Z.  anorg.  1905, 
45.  174.) 

See  also  Ruthenium  nitrosochloride. 

Ruthenium  ^rachloride,  RuCl4. 
Sol.  in  H2O  and  alcohol.    (Glaus.) 

Ruthenium  trichloride  with  MCI. 
See  Chlororuthenite,  M. 

Ruthenium  te^rachloride  with  MCI. 
See  Chlororuthenate,  M. 

Ruthenium    sesgznhydroxide,    Ru2O6H6. 

Sol.  in  acids;  insol.  in  alkalies.  Less  sol. 
in  NH4OH+Aq  than  any  other  oxide  of  the 
Pt  metals.  (Glaus.) 

Ruthenium  ^'hydroxide,   RuO4H4+3H2O. 

Sol.  in  acids  and  alkalies.  (Glaus,  A.  59. 
237.) 

Contains  NO.    Joly,  C.  R.  107.  994.) 

Ruthenium  ^n'odide,  RuI3. 

Ppt.     (Glaus.) 

Insol.  in  H2O,  KI+Aq,  and  aldohol. 
(Gutbier,  Z.  anorg.  1905,  45.  181.) 

Ruthenium  Iniodide  ammonia, 
2RuI3,  7NH3. 

Sol.  in  H2O  and  ammonia  with  slight  warm- 
ing. 

Insol.  in  alcohol.  (Gutbier,  Z.  anoig. 
1905,  45.  182.) 

Ruthenium     nitrosochloride,     RuCl3(NO)  + 

H2O,  and  5H2O. 

Slowly  sol.  in  cold,  easily  in  hot  H2O. 
(Joly,  C.  R.  108.  855.) 

Ruthenium  efthydronitrosochloride, 

NO.Ru2H2Cl3,  2HC1. 

Sol.  in  H2O.  (Brizard,  A.  ch.  1900,  (7) 
21.  353.) 

Ruthenium  silver  nitrosochloride, 
NO.Ru2H2Cl3,  2HC1,  3AgCl. 
Ppt.     (Brizard,  A.  ch.  1900,  (7)  21,  357.) 

Ruthenium    nitrososesom'oxide,   Ru2O3(NO)2 

+2H20. 
Ppt.     (Joly,  C.  R.  108.  854.) 


782 


RUTHENIUM   HYDRONITROSOHYDROXIDE 


Ruthenium  cfthydronitrosohy dioxide, 

NO.Ru2H2(OH)3+2H2O. 
SI.  sol.  in  cold  H2O  with  decomp.     (Briz- 
ard,  A.  ch.  190C,  (7)  21.  349.) 

Ruthenium  cfohydronitrosooxychloride, 

NO.Ru2H2Cl2OH+2H2O. 
Ppt.    (Brizard,  A.  ch.  1900,  (7)  21.  349.) 

Ruthenium  monoxide,  RuO. 

Insol.  in  acids.     (Glaus,  A.  59.  236.) 

Ruthenium  sesgm'oxide,  Ru2O3. 

Insol.  in  acids.  Mixture  of  Ru  and  RuO2. 
(Debray  and  Joly,  C.  R.  106.  1494.) 

See  Ruthenium  nitrososesgwioxide. 

Ruthenium   dioxide,   RuO2. 

Insol.  in  acids.    (Debray  and  Joly.) 

Ruthenium  ^noxide,  RuO3. 

"Ruthenic  acid."    Known  only  in  its  salts. 

Ruthenium  te/roxide,   RuO4. 

Rather  difficultly  and  slowly  sol.  in  H2O. 
(Glaus.) 

Decomp.  in  aqueous  solution  into  Ru2O5  + 
2H2O.  (Debray  and  Joly.) 

Ruthenium  pentoxide,  Ru2O6. 

(Debray  and  Joly,  C.  R.  106.  1494.) 
+2H2O.    Ppt.    (Debray  and  Joly.) 

Ruthenium  heptoxide,  Ru2O7. 

"Pemithenic  acid."  Known  only  in  its 
salts: 

Ruthenium  oxide,  Ru4Os. 
(Debray  and  Joly.) 

Ruthenium  oxychloride,  Ru(OH)Cl2. 

Very  sol.  in  H2O,  but  decomp.  by  an  excess. 
(Joly,  C.  R.  114.  293.) 

Ruthenium  silicide,  RuSi. 

Insol.  in  boiling  acids;  slowly  attacked  by 
a  mixture  of  fused  KHSO4  and  KNO3. 
(Moissan,  C.  R.  1903,  137.  231.) 

Ruthenium  bisulphide,  RuS3. 

Ppt.    (Antony,  Gazz.  ch.  it.  1900,  30.  539.) 

Ruthenomonamine  hydroxide, 

Ru(OH)2(NH3)2+4H2O. 
See  Ruthenosamine  hydroxide. 

Ruthenocfo'amine  carbonate, 

Ru(N2H6)2CO3+5H2O. 
Easily   sol.    in    H2O.      Insol.    in   alcohol. 
(Glaus.) 


Ruthenoc&amine  chloride, 
Ru(N2H6Cl)2+3H2O. 

Not  very  sol.  in  cold,  easily  sol.  in  hot  H2O. 
Insol.  in  alcohol. 

See  Ruthenonitrosocfo'amine    comps. 

—  mercuric  chloride,  Ru(N2H6Cl)2,  HgCl2. 
Nearly  insol.   in   cold,   sol.   in   hot   H2O. 

(Gibbs,  Sill.  Am.  J.  (2)  34,  350.) 

—  chloroplatinate,  Ru(N2H6Cl)2,  PtCl4. 
SI.  sol.  in  H2O.    (Glaus.) 

hydroxide,  Ru(N2H6OH)2. 

Known  only  in  aqueous  solution. 

—  nitrate,  Ru(N2H6NO3)2+2H2O. 
Somewhat  difficultly  sol.  in  cold,  easily  in 

hot  H2O.    Insol.  in  alcohol. 

sulphate,   Ru(N2H6)2SO4+4H2O. 

Moderately  sol.  in  H20.  Insol.  in  alcohol. 
(Glaus.) 

Ruthenocyanhydric  acid,  H4Ru(CN)6. 

Easily  sol.  in  H2O  and  alcohol.  Less  sol. 
in  ether.  (Glaus,  J.  B.  1866.  444.) 

Potassium     ruthenocyanide,     K4Ru(CN)6  + 

3H2O. 

SI.  efflorescent.  Very  sol.  in  H20;  si.  sol. 
in  dil.  alcohol.  (Glaus.) 

Ruthenonitrosocfa'amine  bromide, 

Ru(NO)(NH3)4Br3. 
SI.  sol.  in  H2O.     (Joly,  C.  R.  111.  969.) 
Ru(NO)OH(NH3)4Br2.    Less  sol.  than  cor- 
responding chloride.    (Joly,  C.  R.  108.  300.) 

—  chloride,  Ru(NO)(NH3)4Cl3. 

SI.  sol.  in  H2O.    (Joly,  C.  R.  111.  969.) 
Ru(NO)OH(NH3)4Cl2.      Sol.    in    H2O. 

(Joly,  C.  R.  108.  1300.) 
Ru(NO)(NH3)4Cl3+2H2O  = 

Ru(NO)(OH)(NH3)4Cl2,     HC1+H2O     (?). 

Very  sol.  in  H2O.    (Joly,  C.  R.  111.  969.) 

chloroplatinate, 

Ru(NO)OH(NH3)4PtCl6. 

Scarcely  sol.  in  boiling  H2O.  (Joly,  C.  R. 
108.  1300.) 

Ru(NO)(NH3)4Cl3,  PtCl4.  Ppt.  (Joly, 
C.  R.  111.  969.) 

iodide,  Ru(NO)(NH3)4I3. 

SI.  sol.  in  H2O.    (Joly,  C.  R.  111.  969.) 
Ru(NO)OH(NH3)4I2.     Less  sol.  than  the 

corresponding  bromide.     (Joly,   C.   R.   108. 

1300.) 

•  nitrate,  Ru(NO)(NH3)4(NO3)3. . 

More  sol.  in  H2O  than 

Ru(NO)(OH)(NH,)4(NO8)2.      (Joly,    C.    R. 
111.  969.) 


SCANDIUM   HYDROXIDE 


783 


Ru(NO)OH(NH3)4(NO3)2.  SI.  sol.  in  cold 
H2O;  insol.  in  cone.  HNO3+Aq.  (Joly,  C.  R. 
108.1300.) 

Ruthenonitrosocfaamine  sulphate, 

[Ru(NO)(NH3)4]2(SO4)3  +  10H2O. 

SI.  sol.  in  H2O.    (Joly,  C.  R.  111.  969.) 
[Ru(NO)(NH3)4]4(SO4)6,  H2SO4+H2O.  De- 

comp.  by  cold  H2O.     (Joly.) 

Ru(NO)(OH)4(NH3)4SO4+H2O.  Most  sol. 

in  H2O  of  this  class  of  salts.     (Joly,  C.  R. 

108.  1300.) 

Ruthenonitrous  acid. 

Ammonium      ruthenonitrite,      RuH2(NO2)4, 

3NH4NO2+2H2O. 

Easily  sol.  in  H2O;  practically  insol.  in 
KCl+Aq.  (Brizard,  A.  ch.  1900,  (7)  21. 

368.) 

Potassium  ruthenonitrite, 

K6Ru2(NO2)12  =  6KN02,  Ru2(NO2)3. 

Easily  sol.  in  H2O,  alcohol,  or  ether. 
(Gibbs,  Sill.  Am.  J.  (2),  34.  344.) 

SI.  sol.  in  H2O.  Easily  sol.  in  KNO2+Aq. 
(Glaus.) 

K4Ru2(NO2)io  =  Ru2O2(N2O3)3,    4KNO2. 
Very  sol.  in  H2O.    (Joly  and  Vezes,  C.  R.  109. 
667!) 

K8Ru2(NO2)14  =  Ru2O2(N2O3)2,8KNO2.  SI. 
sol.  in  H2O.  Sol.  in  cold  dil.  acids.  (Joly 
and  Vezes.) 

Ru2H2(NO2)4,  3KNO2+4H2O.  Very  sol. 
in  H2O.  Aqueous  solution  decomp.  si.  on 
long  boiling.  Almost  insol.  in  cone.  KCl-j- 
Aq.  (Brizard,  C.  R.  1899,  129.  216.) 

SUver  ruthenonitrite,  NO.Ru2H2(NO2)4, 

3AgNO2+2H2O. 
Ppt.    (Brizard,  A.  ch.  1900,  (7)  21.  368.) 

Sodium  ruthenonitrite,  Ru2(N02)6,  4NaNO2+ 

4H2O. 

Very  sol.  in  H2O  without  decomp.  (Joly, 
C.  R.  1894,  118.  469.) 

Ruthenosamine  hydroxide, 

Ru(NH3OH)2+4H2O  (?). 
Very  deliquescent,  and  sol.  in  H2O.  (Glaus.) 

Samarium,  Sm. 

The  element  has  not  been  isolated. 

Samarium  bromide,  SmBr3+6H2O.. 
Very  deliquescent.    (Cleve.) 

Samarium  carbide,  SmC2. 

Decomp.  by  water  and  acids.  (Moissan, 
C.  R.  1900,  131.  925.) 


Samarium  bichloride,  SmCl2. 

Decomp.  by  H2O  with  liberation  of  H2  and 
formation  of  samarium  oxide  and  samarium 
oxy  chloride.  Insol.  in  CS2,  CHC13,  benzene, 
abs.  alcohol,  pyridine  and  toluene.  (Matig- 
non,  C.  R.  1906,  142.  85.) 

Samarium  ^nchloride,  SmCl3. 

The  anhydrous  salt  is  very  hydroscopic 
and  easily  sol.  in  H2O.  (Matignon,  C.  R. 
1902,  134.  1309.) 

Very  sol.  in  H2O.  Very  sol.  in  abs.  alcohol. 
6.38  g.  are  sol.  in  100  grams  pyridine  at  ord. 
temp.;  insol.  in  quinoline.  (Matignon,  A.  ch. 
1906,  (8)  8.  406.) 

+3H2O.    Deliquescent. 

Samarium  chloride  ammonia,  SmCl3+NH3; 
+2NH3;     +3NH3;     +4NH3;     +5NH3; 
+8NH3;  +9.5NH3;  +11.5NH3. 
(Matignon,  C.  R.  1905,  140.  143.) 


Samarium  fluoride, 

Precipitate.  Insol.  in  H2O  and  dil.  acids. 
(Cleve.) 

Samarium  iodide,  SmI3. 

(Matignon,  A.  ch.  1906,  (8)  8.  413.) 

Samarium  hydroxide,  Sm2(OH)6. 

Insol.  in  alkalies;  easily  sol.  in  acids,  and 
decomposes  ammonium  salts.  (Cleve,  C.  N. 
61.  145.) 

Samarium  oxide,  Sm2O3. 

Easily  sol.  in  acids.    (Cleve,  C.  N.  51.  145.) 

Samarium  peroxide,  Sm4O9. 
Precipitate.    (Cleve.) 

Samarium  oxy  chloride,  SmOCl. 

(Matignon,  A.  ch.  1906,  (8)  8.  412.) 

Samarium  sulphide,  Sm2S3. 

(Matignon,  A.  ch.  1906,  (8)  8.  415.) 

Scandium,  Sc. 

Element  has  not  been  isolated. 

Scandium    bromide,    Sc2Br6     +3H2O,    and 

+12H20. 
(Crookes,  Roy.  Soc.  Proc.  1908,  80.  A,  518.) 

Scandium    chloride,    Sc2Cl6,     +3H2O,    and 

+  12H2O. 
(Crookes,  Roy.  Soc.  Proc.  1908,  80.  A,  518.) 

Scandium  hydroxide. 

Easily  sol.  in  cone.  HNO3  or  HCl+Aq. 
(Crookes,  Roy.  Soc.  Proc.  1908,  80.  A,  518.) 


784 


SCANDIUM  OXIDE 


Scandium 

oxide,  Sc2O 

3- 

Sp.  gr.  of  H2SeO4+Aq  at  20°  compared  with 

Easily  sol.  by  boiling  with  cone.  HNO3  or 

H2O  at  4°. 

HCl+Aq. 

Wts.  corrected  to  vacuum. 

Scandium 
Decomp 

sulphide,  Sc2S3. 
.  by  H2O  and  by  acids 

with  evolu- 

Sp.  gr. 

% 
H2Se04 

Sp.  gr. 

07            II 

H2Se04  I]  Sp"  gr' 

% 

H2SeO  4 

tion  of  H2S.    (Wirth,  Z.  anorg.  1914,  87.  5.) 

1.000 

1.295 

32.64 

1.590 

54.62 

Selenantimonic  acid. 

1.005 

0^9 

1.300 

33.08 

1.595 

54.92 

Sodium  selenantimonate,  Na3SbSe4+9H2O. 

1.010 
1.015 

1.56 
2.12 

1.305 
1.310 

33.50 
33.92 

1.600 
1.605 

55.28 
55.62 

Sol.  in  2  pts.  cold  H2O.    Insol. 

in  alcohol. 

1.020 

2.92 

.315 

34.36 

1.610 

55.96 

(Hofacker, 

A.  107.  6.) 

1.025 

3.62 

.320 

34.82 

1.615 

56.30 

SI.  sol.  in  H2O;  unstable.     (Pouget,  A.  ch. 

1.030 

4.16 

.325 

35.26 

1.620 

56.60 

1899,  (7)  18.  562.) 

1.035 

4.70 

.330 

35.72 

1.625 

56.88 

Selenantimonous  acid. 

1.040 
1.045 

5.32 
6.08 

.335 
.340 

36.10 
36.43 

1.630 
1.635 

57.20 

57.48 

Potassium 

or//ioselenantimonite.  K3SbSe3. 

1.050 

6.66 

.345 

36.88 

1.640 

57.70 

Ppt.     Decomp.  by 
1  8QQ    (7}  18   560  ) 

H2O.     (Pouget,  A.  ch. 

1.055 
1.060 

7.34 
7.92 

.350 
1.355 

37.34 
37.80 

1.645 
1.650 

58.04 

58.47 

-LOt/i/j    V'/    AO«    *J\J\J*J 

1.065 

8.56 

1.360 

38.24 

1.655 

58.86 

Potassium 

paraselenantimonite, 

K2Sb4Se7  + 

1.070 

9.20 

1.365 

38.66 

1.660 

59.24 

3H2O. 

1.075 

9.82 

1.370 

39.10 

1.665 

59.56 

SI.  sol.  in  H2O;  unstable.     (Pouget,  A.  ch. 

1.080 

10.44 

1.375 

39.50 

1.670 

59.74 

1899,  (7)  18.  560.) 

1.085 

11.02 

1.380 

39.98 

1.675 

59.94 

Sodium     ort/ioselenantimonite, 

Na3SbSe3+ 

1.090 
1.095 

11.62 
12.20 

1.385 
.390 

40.06 
40.66 

1.680 
1.685 

60.18 
60.36 

9H2O. 

1.100 

12.88 

.395 

41.10 

1.690 

60.58 

Very  sol.  in  H2O. 

Aqueous  solution  on 

1.105 

13.58 

.400 

41.56 

1.695 

60.80 

standing  deposits  red  crystals  of  sodium  selen- 

1.110 

14.14 

.405 

41.98 

1.700 

61.06 

antimonate,  Na3SbSe4+9H2O.     (Pouget,  A. 

1.115 

14.66 

.410 

42.36 

1.705 

61.36 

ch.  1899,  (7)  18.  562.) 

1.120 

15.20 

.415 

42.78 

1.710 

.61.64 

Sodium  paraselenantimonite,  Na2Sb4Se7. 

1.125 

15.74 

.420 

43.16 

.715 

61.90 

(Pouget, 

A.  ch.  1899,  (7)  18.  561.) 

.130 
.135 

16.32 
16.86 

.425 
.430 

43.56 
43.94 

.720 
.725 

62.24 
62.48 

Selenic  acid,  H2SeO4. 

.140 

17.38 

.435 

44.32 

.730 

62.76 

Very  sol 

in  H2O  with  evolution  of  heat. 

.145 

17.90 

.440 

44.52 

.735 

63.06 

If  aqueous  solution 

is  evaporated  at  temp. 

.150 

18.44 

.445 

45.00 

.740 

63.32 

of  165°,  acid  has  2.524  sp.  gr.;  at  temp,  of 

.155 

18.92 

.450 

45.32 

.745 

63.60 

267°,  acid 

has  2.60  sp 

gr.;  at  temp,  of  285°, 

1.160 

19.48 

.455 

45.68 

.750 

63.86 

acid  has  2 

.625  sp.  gr. 

Decomp. 

to  H2SeO3 

1.165 

20.02 

.460 

46.04 

.755 

64.04 

at  higher  temp.    (Mitscherlich,  Pogg.  9.  623.) 

1.170 

20.58 

.465 

46.36 

.760 

64.24 

By  evaporation  at  265°,  acid  of  2.609  sp. 

1.175 

21.08 

.470 

46.70 

1.765 

64.42 

gr.  containing  95%  H2SeO4  is  obtained.     If 

1.180 

21.60 

.475 

47.01 

1.770 

64.62 

brought  at 

same  temp 

.  in  vacuo  over  H2SO4, 

1.185 

22.22 

.480 

47.32 

1.775 

64.84 

acid  of  2.627  sp.  gr.'with  97.5% 

H2SeO4  is 

1.190 

22.66 

1.485 

47.66 

1.780 

65.06 

obtained  . 

(Fabian,  A 

Suppl.  1.  243.) 

1.195 

23.18 

1.490 

47.98 

1.785 

65.28 

Sp.gr.  of  H2Se04+Aq. 

1.200 
1.205 

23.70 
24.26 

1.495 
1.500 

48.28 
48.54 

1.790 
1.795 

65.48 
65.66 

%  H2Se04 

Sp.  gr. 

%  H2SeO4 

Sp.  gr. 

1.210 

24.84 

1.505 

48.92 

1.800 

65.90 

1.215 

25.30 

1.510 

49.30 

1.805 

66.12 

99.73 

2.6083 

90.0 

2.3848 

1.220 

25.84 

1.515 

49.68 

1.810 

66.36 

99.50 

2.6051 

89.0 

2.3568 

1.225 

26.30 

1.520 

50.02 

1.815 

66.64 

99.00 

2.6975 

88.0 

2.3291 

1.230 

26.84 

1.525 

50.34 

1.820 

66.90 

98.5 

2.5863 

87.0 

2.3061 

1.235 

27.28 

1.530 

50.68 

1.825 

67.16 

98.0 

2.5767 

86.0 

2.2795 

1.240 

27.70 

1.535 

51.04 

1.830 

67.46 

97.5 

2.5695 

85.0 

2.5558 

1.245 

28.18 

1.540 

51.38 

1.835 

67.72 

97.0 

2.5601 

84.0 

2.2258 

1.250 

28.58 

1.545 

51.66 

1.840 

68.02 

96.0 

2.5388 

83.0 

2.1946 

1.255 

29.06 

1.550 

51.98 

1.845 

68.30 

95.0 

2.5163 

82.0 

2.1757 

1.260 

29.44 

1.555 

52.28 

1.850 

68.50 

94.0 

2.4925 

81.0 

2.1479 

.265 

29.82 

1.560 

52.56 

1.855 

68.70 

93.0 

2.4596 

80.0 

2.1216 

.270 

30.26 

1.565 

52.88 

1.860 

68.92 

92.0 

2.4322 

79.0 

2.0922 

.275 

30.76 

1.570 

53.28 

1.865 

69.12 

91.0 

2.4081 

73.50 

1.9675 

.280 

31.26 

1.575 

53.56 

1.870 

69.34 

.285 
1.290 

31.74 
32.18 

1.580 
1.585 

53.94 
54.30 

1.875 
1.880 

69.56 
69.72 

(Cameron  and  Macallan,  Lond.  R 
46.  13.) 

Soc.  Proc. 

SELENATE,  AMMONIUM   CADMIUM 


785 


Sp.  gr.  of  H2SeO4+Aq—  Concluded. 

Selenates. 

All  the  neutral  and.  acid  salts  of  H2SeO4  arc 

Sp.  gr. 

% 

H2SeO4 

Sp.   gr. 

% 

H2Se04 

Sp.  gr. 

% 

H2SeO4 

sol.  in  H2O,  except  BaSeO4,  SrSeO4,  CaSeO4, 
and  PbSeO4,  which  are  nearly  or  quite  insol. 
inH2O  orHNOs+Aq. 

1.885 

69.94 

2.125 

80.25 

2.365 

89.14 

1.890 
1.895 

70.14 
70.38 

2.130 
2.135 

80.42 
80.68 

2.370 
2.375 

89.30 
89.48 

Aluminum  selenate,  Al2(SeO4)3. 

1.900 

70.64 

2.140 

80.74 

2.380 

89.60 

.  Resembles  in   every  way  aluminum  sul- 

1.905 

70.78 

2.145 

80.96 

2.385 

89.72 

phate.    (Berzelius.) 

1.910 

71.00 

2.150 

81.14 

2.390 

89.84 

1.915 

71.21 

2.155 

81.36 

2.395 

89.96 

Aluminum  ammonium  selenate, 

1.920 

71.38 

2.160 

81.60 

2.400 

90.10 

Al2(NH4)2(SeO4)4+24H2O. 

1.925 
1.930 
1.935 

71.68 
72.00 

72.38 

2.165 
2.170 
2.175 

81.80 
82.02 

82.22 

2.405 
2.410 
2.415 

90.20 
90.30 
90.46 

More  sol.  in  H2O  than  the  corresponding 
sulphate.    (Wohlwill,  A.  114.  191.) 

1.940 
1.945 

72.66 

72.88 

2.180 
2.185 

82.44 
82.64 

2.420 
2.425 

90.74 
91.00 

Aluminum  caesium  selenate,  Al2Cs2(SeO4)4+ 

1.950 

73.12 

2.190 

82.78 

2.430 

91.24 

24H2O. 

1.955 

73.34 

2.195 

82.96 

2.435 

91.46 

(Peterson,  B.  9.  1563.) 

1.960 

73.54 

2.200 

83.10 

2.440 

91.70 

Much  more  sol.  in  H2O  than  the  corre- 

1.965 

73.74 

2.205 

83.24 

2.445 

92.00 

sponding  sulphate.    (Fabre,  C.  R.  105.  114.) 

1.970 

73.98 

2.210 

83.44 

2.450 

92.28 

1.975 
1.980 

74.22 
74.44 

2.215 
2.220 

83.62 

83.78 

2.455 
2.460 

92.56 
92.85 

Aluminum  potassium  seJenate,  Al2K2(SeO4)4 
+24H2O. 

1.985 
1.990 

74.66 

74.86 

2.225 
2.230 

83.96 
84.14 

2.465 
2.470 

93.02 
93  .  20 

More   sol.   in   H2O   than   common   alum. 

1.995 

75.08 

2.235 

84.30 

2.475 

93.36 

(Weber,  Pogg.  108.  615.) 

2.000 

75.28 

2.240 

84.48 

2.480 

93.68 

2.005 

75.46 

2.245 

84.60 

2.485 

94.02 

Aluminum  rubidium  selenate,  Al2Rb2(SeO4)4 

2.010 

75.66 

2.250 

84.82 

2.490 

94.32 

+24H2O. 

2.015 

75.88 

2.255 

85.02 

2.495 

94.48 

(Peterson,  B.  9.  1563.) 

2.020 

76.06 

2.260 

85.26 

2.500 

94.64 

Much  more  sol.  in  H2O  than  the  corre- 

2.025 
2.030 

76.14 
76.48 

2.265 
2.270 

85.44 
85.60 

2.505 
2.510 

94.80 
94.96 

sponding  sulphate.    (Fabre,  C.  R.  105.  114.) 

2.035 
2.040 

76.68 
76.84 

2.275 

2.280 

85.78 
85.96 

2.515 
2.520 

95.32 
95.58 

Aluminum  sodium  selenate,  Al2Na2(SeO4)4  + 

94.TT  O 

2.045 
2.050 

77.08 
77.36 

2.285 
2.290 

86.16 
86.38 

2.525 
2.530 

95.86 
96.10 

<i^txl2vy. 

SI.  efflorescent.    Very  sol.  in  H2O.    (Wohl- 

2.055 

77.50 

2.295 

86.60 

2.535 

96.41 

will,  A.  114.  191.) 

2.060 

77.62 

2.300 

86.82 

2.540 

96.68 

2.065 

77.80 

2.305 

87.04 

2.545 

96.92 

Aluminum  thallium  sulphate,  Al2Tl2(SeO4)4  + 

2.070 

78.06 

2.310 

87.26 

2.550 

97.12 

24H2O. 

2.075 

78.24 

2.315 

87.46 

2.555 

97.30 

Sol.  in  H2O.    (Fabre,  C.  R.  105.  114.) 

2.080 

78.48 

2.320 

87.66 

2.560 

97.48 

2.085 
2.090 
2.095 
2.100 

78.68 
78.84 
79.08 
79.28 

2.325 
2.330 
2.335 
2.340 

87.84 
88.00 
88.18 
88.34 

2.565 
2.570 
2.575 
2.580 

97.68 
97.94 
98.20 
98.46 

Aluminum     selenate     potassium     sulphate, 
Al2(SeO4)3,  K2SO4+24H2O. 
Sol.  in  H2O.    (v.  Gerichten,  A.  168.  222.) 

2.105 
2.110 

79.50 

79.68 

2.345 
2.350 

88.48 
88.66 

2.585 
2.590 

98.70 
99.04 

Ammonium  selenate,  (JNH4)2SeO4. 

2.115 

79.90 

2.355 

88.82 

2  .  595 

99.36 

Easily  sol.  in  H2O. 

2.120 

80.10 

2.360 

88.98 

100  g.  H2O  dissolve  117  g.  (NH4)2SeO4  at 

7°;  164  g  at  59°;  197  g.  at  100°.    (Tutton 

(Diemer  and  Lenher.  J.  phys.  Chem.  1909, 
13    ^OQ  t 

Proc.  Roy.  Soc.  1907,  79,  A.  351.) 
Insol.  in  liquid  NH3.     (Franklin,  Am.  Ch. 

Aw»   *j\j*y»J 

J.  1898,  20.  826.) 

Sol.  in  cone,  or  fuming  ,H2SO4. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  830.) 

Decomp.  by  alcohol. 

+H2O.  (Cameron  and  Macallan,  C.  N. 
59.  232.) 

+2H2O,  and  +6H2O  (?).    (C.  and  M.) 

+4H20.  (Kremann  and  Hofmeier,  M. 
1908,  29. 1117.) 


Ammonium  hydrogen  selenate,  NH4HSeO4. 
Sol.  in  H2O.    (Topsoe.) 

Ammonium  cadmium  selenate,  (NH4)2SeO4, 

CdSeO4+2H2O. 

Sol.  in  H2O.    (Topsoe,  W.  A.  B.  66,  2.  2.) 
+6H2O.    Efflorescent.    Very  easily  sol.  in 

H2O.    (Topsoe.) 


786 


SELENATE,  AMMONIUM  CEROUS 


Ammonium  cerous  selenate, 

(NH4)2Ce2(SeO4)4+9H2O. 
Easily  sol.  in  H2O.    (Jolin.) 

Ammonium  chromium  selenate, 

(NH4)2Cr2(SeO,),+24H2O. 
Sol.  inH2O.    (Fabre,  C.  R.  105.  114.) 

Ammonium  cobaltous  selenate,  (NH4)2SeO4, 

CoSeO4+6H2O. 
Easily  sol.  in  H2O.    (Topsoe.) 

i    cupric 

CuSeO4+6H2O. 
Sol.  in  H2O.    (Topsoe.) 

Ammonium  didymium  selenate,  (NH4)2SeO4, 

Di2(SeO4)3+6H2O. 
Easily  sol.  in  H2O.    (Cleve.) 
+10H2O.    (Cleve,  Bull.  Soc.  (2)  43.  363.) 

Ammonium    erbium    selenate,    (NH4)2SeO4, 

Er2(SeO4)3+4H2O. 
Easily  sol.  in  H2O.    (Cleve.) 

Ammonium  ferrous  selenate,  (NH4)2Fe(SeO4)2 

+6H2O. 

Easily  sol.  in  H2O.    (Topsoe.) 
+2H2O. 

Ammonium  lanthanum  selenate,  (NH4)2SeO4, 

La2(SeO4)3-f9H2O. 
Sol.  inH2O.    (Cleve.) 

Ammonium  magnesium  selenate, 

(NH4)2Mg(SeO4)2+6H2O. 
Easily  sol.  in  H2O.    (Topsoe.) 

Ammonium  manganous  selenate,  (NH4)2SeO4, 

MnSeO4+6H2O. 

Not    deliquescent.      Easily    sol.    in    H2O. 
(Topsoe.) 

Ammonium    nickel    selenate,     (NH«)2SeO4. 

NiSe04+6H20. 
Sol.  in  H2O.    (Topsoe.) 

Ammonium  samarium  selenate,  (NH4)2SeO4, 

Sm2(SeO4)3+6H2O. 
Easily  sol.  in  H2O.    (Cleve.) 

Ammonium  thallium  selenate,   (NH4)2SeO4, 

Tl2(Se04)3+8H20. 
Sol.  in  H2O.    (Fortini,  C.  C.  1903,  II.  706.) 

Ammonium    uranyl    selenate,    (NH4)2SeO4 

(UO2)SeO4+2H2O. 
Easily  sol.  in  H2O.    (Sendtner.) 

Ammonium   yttrium   selenate,    (NH4)2SeO4 

Y2(SeO4)3+6HO. 
Very  sol.  in  F2O.    (Cleve.) 


Ammonium  zinc  selenate, 

(NH4)2SeO4,  ZnSeO4+6H2O. 
Sol.  in  H2O.    (Topsoe.) 

Antimony  selenate. 

Insol.  in  H2O.  Not  very  sol.  in  acids.  Sol. 
in  H2SeO4.  (Cameron  and  Macallan.) 

Barium  selenate,  BaSeO4. 

Somewhat  more  sol.  in  H2O  and  dil.  acids 
than  BaSO4.  (Rose.)  100  ccm.  H2O  dissolve 
11.8  mg.  in  the  cold,  and  13.8  mp.  at  100°. 
(Petersson,  Z.  anal.  12.  287.) 

Not  decomp.  by  H2SO4.  Insol.  in  HNO3  + 
Aq  (Berzelius),  but  decomp.  by  solution  of 
alkali  carbonates  at  ordinary  temp. 

Very  slowly  decomp.  by  HCl+Aq.  (Rose, 
Pogg.  95.  426.) 

Bismuth  selenate. 

Insol.  in,  and  not  decomp.  by  cold  or  hot 
H2O.  (Cameron  and  Macallan.) 

Caesium  selenate,  Cs2SeO4. 

Sol.  in  H2O.    (Petersson,  B.  9.  1561.) 

IOC  g.  H2O  at  12°  dissolve  244.8  g.  Cs2SeO4. 

(Tutton,  Chem.  Soc.  1897,  71.  850.) 

Sp.  gr.  of  Cs2SeO4+Aq  at  20°  compared 

with  H2O  at  4°,  containing: 

%  Cs2SeO4  45.94          53.43 

Sp.gr.  1.5841         1.7432 

(Tutton.) 

Caesium  hydrogen  selenate,  CsHSeO4. 

Ppt.  Very  hygroscopic.  (Norris,  Am.  Ch. 
J.  1901,  26.  322.) 

Caesium  chromic  selenate,   Cs2Cr2(SeO4)4  + 

24H2O. 
Sol.  mH2O.    (Fabre,  C.  R.  105.  114.) 

Caesium  cobaltous  selenate,  Cs2Co(SeO4)2  + 

6H2(X 
Sol.  in  H2O.    (Topsoe.) 

Caesium    indium     selenate,     CsIn(SeO4)2  + 

12H2O. 

Efflorescent;  sol.  in  H2O.  (Mathers,  J. 
Am.  Chem.  Soc.  1908,  30.  215.) 

Caesium  iron  (ferric)  selenate,  Cs2Fe2(SeO4)4 

+24H2O. 

SI.  sol.  in  H2O.  (Roncogliolo,  Gazz.  ch. 
it.  1905,  35.  (2)  553.) 

Caesium     magnesium      selenate,     Cs2SeO4, 
MgSe04+6H2O. 
(Tutton,  Chem.  Soc.  1905,  87,  1163.) 

Caesium  zinc  selenate,  Cs2Zn(SeO4)2+6H2O. 
(Tutton,  Zeit.  Kryst.  1900,  33.  14.) 


SELENATE,   CUPRIC  HYDRAZINE 


787 


Cadmium  selenate,  CdSeO4+2H2O. 

Very  sol.  in  H2O.    (v.  Hauer,  W.  A.  B.  39. 
299.) 

Cadmium  potassium  selenate.  CdSeO4,  K2SO4 

+2H20. 

Sol.  in  H2O;  can  be  recrystallized  without 
decomp.    (v.  Hauer,  W.  A.  B.  54.  209.) 

Calcium  selenate,  CaSeO4+2H2O. 

Less  sol.  in  hot  than  in  cold  H2O.      (v. 
Hauer,  J.  pr.  80.  214.) 

Sat.  CaSeO4+Aq  contains  at: 
— 1°        +5°       20°        37°        67° 
7.4          7.3         7.6        6.8        5.1%  CaSeO4. 
Cfitard,  A.  ch.  1894,  (7)  2.  551.) 

Cerous  selenate,  Ce2(SO4)3+6H2O,  9H2O,  or 
12H20. 

More  sol.  in  cold  than  hot  H2O.    (Jolin.) 

+4H2O.    Very  easily  in  cold,  si.  sol.  in  hot 
H2O.    (Cingolani,  C.  C.  1908, 1.  1606.) 

Stable  above  100°. 

+5H2O.    Stable  at  92-100°. 

+7H2O.    Stable  at  80-92°. 

+8H2O.    Stable  at  50-78°. 

+10H2O.    Stable  at  34-40°. 

+11H2O.    Stable  at  12-28°. 

+12H2O.   Stable  at  0-12°.    (Cingolani,  C. 
A.  1908.  2658.) 

Solubility  of  Ce2(SeO4)3  in  H2O  at  t°. 

(G.  salt  calculated  as  anhydrous  Ce2(SO4)3 

dissolved  in  100  cc.  H2O.) 


t° 

£§q 

1 

t° 

1 

^ 

bflO  O 
C3  o^ 

gp 

4.*56 

1^785 
2.513 

0° 
11.6 
12.6 
26.6 
28.8 
34.2 
45.6 
45.9 

37" 

33^84 

33^15 
32.16 

39.55 
36.'6 
33.2 

3L89 

60° 
60.8 
78.2 
80.5 
91 
95.4 
98 
100 

13.68 
5^52 

2.'02 
1.53 

(Cingolani,  I.  c.) 

Cerous     potassium     selenate,     Ce2(SeO4)3, 
5K2SeO4. 
More  sol.  in  H2O  than  the  corresponding 
sulphate.    (Jolin.) 

Cerous  sodium  selenate,  Ce2(SeO4)3,  Na2SeO4 

+5H2O. 
Quite  sol.  in  H2O.    (Jolin.) 

Chromic  potassium  selenate,  Cr2K2(SeO4)4+ 

24H2O. 
Resembles  the  sulphate  in  every  particular. 


Chromic  rubidium  selenate,  Cr2Rb2(SeO4)4  + 

24H2O. 
Sol.  in  H2O. 

Chromic  sodium  selenate,  Cr2Na2(SeO4)4-f- 

24H2O. 
Sol.  in  H2O.    (Fabre,  C.  R.  105.  114.) 

Chromic  thallous  selenate,  Cr2Tl2(SeO4)4+ 

24H2O. 
Sol.  in  H2O.    (Fabre,  C.  R.  105.  114.) 

Chromic  selenate  potassium  sulphate, 

Cr2(SeO4)3,  K2SO4+24H2O. 
Sol.  in  H2O.    (v.  Gerichten.) 

Cobaltous  selenate,  basic,  4CoO,  3SeO3  + 
H20. 

Insol.  in  H2O;  sol.  in  acids.  (Bogdan,  Bull. 
Soc.  (3)  9.  586.) 

Co3(OH)2(SeO4)3.  Insol.  in  H2O.  Sol.  in 
acids.  (Bogdan,  C.  C.  1895.  630.) 

Cobaltous  selenate,  CoSeO4+5H2O. 
Easily  sol.  in  H2O.    (Topsoe.) 
+6H2O.    Easily  sol.  in  H2O.    (Topsoe.) 
+7H2O.     Efflorescent.     Extremely  sol.  in 

H2O.    (Topsoe.) 

+  18H2O.     Very  unstable.      (Copaux,   A. 

ch.  1905,  (8)  6.  553.) 

Cobaltous  potassium  selenate,  CoSeO4, 

K2SeO4+6H2O. 

More  sol.  in  H2O  than  corresponding  sul- 
phate. (v.  Hauer,  W.  A.  B.  39.  837.) 

Cobaltous  rubidium  selenate,  CoRb2(SeO4)2 

+6H2O. 
Sol.  in  H2O.    (Topsoe.) 

Cobaltous  thallous  selenate,  CoTl2(SeO4)2+ 

6H2O. 
Sol.  in  H2O.    (Topsoe.) 

Cupric  selenate,  basic,  3CuO,  2SeO3+4H2O. 

Insol.  in  H2O;  sol.  in  acids.  (Bogdan,  Bull. 
Soc.  (3)  9.  588.) 

+5H2O.  SI.  sol.  in  cold  H2O.  (Metzner, 
C.  R.  1898,  127.  55.) 

Cupric  selenate,  CuSeO4+5H2O. 

Solubility  in  H2O:— 

257  g.  salt  in  1  1.  sat.  solution  at  15°. 

346  '•    "     "  1  1.  "  "        "  35°. 

435  "    "     "  11.  "          "        "  55°. 

Aq.  solution  decomp.  at  70°.  (Metzner, 
C.  R.  1898,  127.  55.) 

+H2O,  and  +2H20.    (Metzner.) 

Cupric    hydrazine    selenate,    N2H4.H2SeO<, 


Decomp.  in  aq.  solution.     (Rimini,  C.  C. 
1907,  I.  86.) 


788 


SELENATE,   CUPRIC  MAGNESIUM 


Cupric  magnesium  selenate,  CuMgs(SeO4)4+ 

28H20. 
Sol.  inH2O.    (Wohlwill.) 

Cupric  nickel   selenate,   CuSeO4,   NiSeO4+ 

14H2O. 
Sol.  inH2O.    (Wohlwill.) 

Cupric  potassium  selenate,  CuSeO4,  K^SeO4  + 

6H2O. 
SI.  sol.  in  H2O.    (Topsoe.) 

Cupric  zinc  selenate,  CuZn3(SeO4)4+28H2O. 
Sol.  inH2O.    (Wohlwill.) 

Cupiic  selenate  ferrous  sulphate,  2CuSeO4, 

3FeSO4+35H2O. 
Sol.  in  H2O.    (Wohlwill.) 

Cupiic  selenate  magnesium  sulphate,  CuSeO4, 

3MgSO4+28H2O. 
Sol.  in  H2O.    (Wohlwill.) 

Cupric    selenate    zinc     sulphate,     CuSeO4, 

3ZnSO4+28H2O. 
Sol.  inH20.    (Wohlwill.) 

Didymium  selenate,  Di2(SeO4)3+5H2O,  and 

6H20. 

Sol.  in  H2O. 

+8H2O.    Easily  sol.  in  H2O.    (Cleve.) 
+  10H2O.    Sol.  inH2O.    (Cleve.) 

Didymium  potassium   selenate,   Di2(SeO4)3, 

K2SeO4+9fl2O. 

Not    deliquescent.      Easily   sol.   in   H2O. 
(Cleve.) 

Didymium     sodium     selenate,     Di2(SeO4)3, 

Na2SeO4+4H2O. 
Easily  sol.  in  H2O.    (Cleve.) 

Dysprosium  selenate,  Dy2(SeO4)3+8H20. 

Easily    sol.    in    H2O;    insol.    in    alcohol. 
(Jantsch,  B.  1911,  44.  1275.) 

Erbium    selenate,    Er2(SeO4)3+8H2O,    and 

9H2O. 
Easily  sol.  in  H2O.    (Topsoe.) 

Erbium  potassium  selenate,  Er2(SeO4)3, 

K2SeO4+8H2O. 
Easily  sol.  in  H2O.    (Cleve.) 

Gadolinium  selenate,  Gd2(SeO4)3  +  10H2O. 

Decomp.  in  the  air.    (Benedicks,  Z.  anorg. 
1900,  22.  410.) 

Gadolinium  potassium  selenate,  Gd2(SeO4)3, 

3K2Se04+4H20. 

Sol.  in  H2O.     (Benedicks,  Z.  anorg.  1900, 
22.  412.) 


Glucinum  selenate,  GlSeO4+4H2O. 
Very  sol.  in  H2O.    (Atterberg.) 

Gold  (auric)  selenate,  Au2(SeO4)3. 

Insol.  in  H2O.  Sol.  in  hot  cone.  H2SeO4+ 
Aq.  Somewhat  sol.  in  H2SO4  and  HNO3-|- 
Aq.  Decomp.  by  HCl+Aq.  (Lenher,  J.  Am. 
Chem.  Soc.  1902,  24.  355.) 

Indium  selenate,  In2(SeO4)3  +  10H2O. 

Hydroscopic;  easily  sol.  in  H2O.  (Mathers. 
J.  Am.  Chem.  Soc.  1908,  30.  214.) 

Iron  (ferrous)  selenate,  FeSeO4-f5H2O. 
Sol.  in  H2O.  (Wohlwill,  A.  114.  169.) 
+7H2O.  Efflorescent,  and  sol.  in  H2O. 

(Topsoe.) 

Iron  (ferrous)  potassium  selenate,  FeSeO4, 

K2SeO4+6H2O. 

Easily  sol.  in  H2O.  Solution  decomp.  some- 
what on  standing.  (Topsoe.) 

Iron  (ferric)  rubidium  selenate,  Rb2Fe2(SeO4)4 

+24H2O. 

SI.  sol.  in  H2O.  (Roncogliolo,  Gazz.  ch.  it. 
1905,  35.  (2)  553.) 

Iron    (ferric)    selenate   potassium   sulphate, 

Fe2(SeO4)3,  K2SO4+24H2O. 
Sol.  in  H2O.    (v.  Gerichten.) 

Lanthanum  selenate,  La2(SeO4)3+6H2O,  and 

10H2O. 

Easily  sol.  in  cold  H2O.    (Cleve.) 
+  12H2O.     (Frerichs  and  Smith,  A.   191. 

355.) 

Lanthanum  potassium  selenate,  La2(SeO4)3, 

K2SeO4+9H2O. 
Quite  sol.  in  H2O.    (Cleve.) 

Lanthanum    sodium    selenate,    La2(SeO4)3, 

Na2SeO4+4H2O. 
Easily  sol.  in  H2O.    (Cleve.) 

Lead  selenate,  basic,  2PbO,  SeO8. 

Decomp.  by  acids  with  separation  of 
PbSeO4. 

3PbO,  PbSeO4+H2O.  Ppt.  (Stromholm, 
Z.  anorg.  1904,  38.  443.) 

Lead  selenate,  PbSeO4. 

Insol.  in  H2O  or  HNO3+Aq.  (Schafarik, 
W.  A.  B.  47.  256.) 

Min.  Kerstenite. 

Lithium  selenate,  Li2SeO4+H2O. 

Not  deliquescent.  Easily  sol.  in  H2O. 
.(Topsoe.) 


SELENATE,   POTASSIUM,   ALUMINUM   SULPHATE 


789 


Magnesium  selenate,  MgSeO4+6H2O. 

Solubility  resembles  closely  that  of  MgSO4. 
(Topsoe.) 

Magnesium  potassium  selenate,  MgK2(SeO4)2 

+6H2O. 
Easily  sol.  in  H2O.    (Topsoe.) 

Magnesium    rubidium     selenate,     MgSeO4, 

Rb2SeO4+6H2O. 
(Tutton,  Chem.  Soc.  1905,  87.  1163.) 


Manganous  selenate,  MnSeO,+2H2O. 

Easily  sol.  in  H2O.    (Topsoe.) 

+5H2O.     Easily  sol.   in  H2O.     Solution 
decomp.  on  warming  or  standing.     (Topsoe.) 


Ma 


nganous 
MnSeO4. 


s    potassium    selenate,    K2SeO4, 


Not  deliquescent.  Easily  sol.  in  H2O. 
(Topsoe.) 

Mercurous  selenate,  6Hg2O,  5SeO3. 

Very  si.  sol.  in  H2O.  SI.  attacked  by  boil- 
ing HNO3.  Insol.  in  HCl+Aq.  (Kohler, 
Pogg.  89.  146.) 

Hg2SeO4.  Very  si.  sol.  in  H2O;  insol.  in 
HCl+Aq.  (Cameron  and  Davy,  C.  N.  44. 
63.) 

Mercuric  selenate,  basic,  6HgO,  2SeO3+H2O. 

Insol.  in  H2O,  or  cold  HNO3+Aq.  Sol.  in 
hot  HNO3  or  HCl+Aq.  (Kohler.) 

HgSeO4,  2HgO.  Sol.  in  10,330  pts.  H2O. 
(Cameron  and  Davy.) 

Mercuric  selenate,  HgSeO4+H2O. 

Decomp.  by  H2O  with  formation  of  basic 
salt.  (Kohler.) 

Sol.  in  H2SeO4,  H2SO4,  HNO3,  or  HCl+Aq, 
but  decomp.  by  H2O  to  2HgO,  HgSeO4. 
(Cameron  and  Davy,  C.  N.  44.  63.) 

Nickel  selenate,  NiSeO4+6H2O. 

Very  easily  sol.  in  H2O.  (v.  Hauer,  W.  A. 
B.  39.  305.) 

Nickel  potassium  selenate,  NiSeO4,  K2SeO4  + 

6H2O. 
Sol.  in  H2O.    (Topsoe.) 

Nickel  thallium  selenate,  NiSeO4,  Tl2SeO4  + 

6H2O. 
Sol.  in  H2O.    (Petersson.) 

Platinum  selenate. 

Sol.  in  boiling  H20.  Sol.  in  HCl+Aq. 
Insol.  in  alcohol.  (Cameron  and  Macallan, 
Lond.  R.  Soc.  Proc.  46.  13.) 


Potassium  selenate,  K2SeO4. 

Nearly  equally  sol.  in  cold  and  hot  H2O. 
(Mitscherlich,  Pogg.  9.  623.) 

100  g.  H2O  dissolve  110.5  g.  K2SeO4  at  0°; 
112.8  g.  at  20°;  122.2  g.  at  100°.  (Etard, 
C.  R.  1888,  106.  741.) 

Sat.  K2SeO4+Aq  contains  at: 
—20°        —5°         +5° 
51.5          51.7         52.0%  K2SeO4, 

18°          97° 

52.6        54.9%  K2SeO4. 
(Etard,  A.  ch.  1894,  (7)  2.  550.) 

100  g.  H2O  at  12°  dissolve  115.0  g.  K2SeO4. 
(Tutton,  Chem.  Soc.  1897,  71.  850.) 

Sp.  gr.  of  K2SeO4+Aq  at  20°  compared 
with  H2O  at  4°,  containing: 
%K2SeO4  35.76         41.79         50.00 

Sp.  gr.  1.3591        1.4385        1.5590 

(Tutton,  Chem.  Soc.  1897,  71.  851.) 

Potassium  hydrogen  selenate,  KHSeO4. 
Sol.  in  H2O. 

Potassium  praseodymium  selenate,  3K2SeO4, 

Pr2(SeO4)3+4H2O. 

SI.  sol.  in  H2O.  (von  Scheele,  Z.  anorg. 
1898,  18.  361.) 

Potassium  samarium  selenate,  K2Se04, 

Sm2(SeO4)3+6H2O. 

Easily  sol.  in  H2O.  (Cleve,  Bull.  Soc.  (2) 
43.  166.) 

Potassium   sodium   selenate,   3K2SeO«, 

Na2SeO4. 
Sol.  inH2O.    (Topsoe.) 

Potassium   thallium   selenate,   K2SeO4, 

Tl2(Se04)3+8H20. 

Very  sol.  in  dil.  acids.  (Fortini,  C.  C.  1903, 
II.  706.) 

Potassium  uranyl  selenate,  K2SeO4, 

(U02)Se04+2H20. 

SI.  sol.  in  cold,  easily  in  hot  H2O.  (Sendt- 
ner.) 

Potassium  yttrium  selenate,  K2SeO4, 

Y2(SeO4)3+6H2O. 
Very  sol.  in  H2O.    (Cleve.) 

Potassium  zinc  selenate,  K2SeO4,  ZnSeO4  + 

2H2O. 

Sol.  in  H2O.    (Topsoe.) 
+6H2O.    Sol.  in  H2O.    (Topsoe.) 

Potassium     selenate     aluminum     sulphate, 

K2SeO4,  A12(SO4)3+24H2O. 
Sol.  in  H2O.    (v.  Gerichten.) 


790 


SELENATE,   POTASSIUM,   CHROMIC  SULPHATE 


Potassium   selenate   chromic    sulphate, 

Solubility  in  H2O  at  t°. 

K2SeO4,  Cr2(SO4)3+24H2O. 

Sol.  in  H2O.    (v.  Gerichten.) 

t° 

%  Na2Se04 

Mols.  H2O 
to  1  mol. 

Mols.  anhy- 
drous salt  to 

Na2SeO4 

100  mols.  H2O 

Potassium  selenate  ferric  sulphate,  K2SeO4, 

Fe2(SO4)3+24H2O. 
Sol.  in  H2O.    (\.  Gerichten.) 

35.2 
39.5 
50 

45.47 
45.26 
44.49 

12.59 
12.70 
13.10 

7.94 

7.87 
7.63 

75 

42.83 

14.00 

7.14 

Potassium    selenate    manganous    sulphate, 

100 

42.14 

14.42 

6.93 

K2SeO<,  MnSO4+6H2O. 

Sol.  in  H2O.    (v.  Gerichten,  A.  168.  225.) 

(Funk,  B.  1900,  33.  3697.) 

Potassium  selenate  manganic  sulphate, 

+  10H2O.    Solubility  in  H2O  at.t°. 

K2SeO4,  Mn2(SeO4)3+24H2O. 
Sol.  in  H2O.    (v.  Gerichten.) 

t° 

%  Na2SeO4 

Mols.  H2O 
to  1  mol. 

Mols.  anhy- 
drous salt  to 

Na2SeO4 

100  mols.  H20 

Praseodymium  selenate,  Pr2(SeO4)2. 

o 

11.74 

79  08 

1  26 

Sol.  in  H2O.     (von  Schule,  Z.  anorg.  1898, 

15 

25.01 

31.  '48 

3^18 

18.  360.) 
+8H2O.    SI.  sol.  in  H2O;  sol.  in  H2SO4. 

25.2 

27 

36.91 
39.18 

17.95 
16.30 

5.57 
6.13 

(von  Schule.) 

30 

44.05 

13.33 

7.50 

Rubidium  selenate,  Rb2SeO4. 

Sol.  in  H2O.    (Petersson.) 

IOC  g.  H2O  at  12°  dissolve  158.9  g.  Rb2SeO4. 
(Tutton,  Chem.  Soc.  1897,  71.  850.) 

Sp.  gr.  of  Rb2SeO4+Aq  at  20°  compared 
with  H2O  at  4°,  containing: 

%  Rb2SeQ4  40.60          47.07 

Sp.  gr.  .        1.4688         1.5806 

(Tutton.) 

Rubidium  hydrogen  selenate,  RbHSeO4. 

Sol.  in  equal  pts.  H2O;  very  hydroscopic. 
(Norris,  Am.  Ch.  J.  1901,  26.  321.) 

Rubidium    zinc    selenate,     Rb2Zn(SeO4)2  + 

6H2O. 
(Tutton,  Zeit.  Kryst.  1900,  33.  8.) 

Samarium  selenate,  Sm2(SeO4)3+8H2O. 
More  sol.  in  H2O  than  Sm2(SO4)3. 
+  12H2O.    Efflorescent.    (Cleve.) 

Scandium   selenate,  Sc2(SeO4)3+2H2O,  and 

+8H2O. 

rCrookes,  Roy.  Soc.  Proc.  1908,  80,  A. 
518.) 

Silver  selenate,  Ag2SeO4. 

As  Ag2SO4.    (Mitscherlich,  Pogg.  12.  138.) 

Silver  selenate  ammonia,  Ag2SeO4,  4NH3. 

Easily  sol.  in  H2O  or  ISH4OH+Aq  without 
decomp.  (Mitscherlich,  Pogg.  12.  141.) 

Sodium  selenate,  Na2SeO4. 

Very  sol.  in  H2O,  forming  supersat.  solu- 
tions. Cryst.  also  with  10H2O,  which 
effloresce.  Maxinrum  point  of  solubility  is 
at  33°.  (Mitscherlich.) 


(Funk.) 

Sp.  gr.  of  sat.  solution  at  18°  =  1.315. 
(Funk.) 

Sodium  selenate  vanadate. 
See  Selenovanadate,  sodium. 

Strontium  selenate,  SrSeO4. 

Insol.  in  H2O  or  HNO3+Aq;  decomp.  by 
long  boiling  with  HCl+Aq. 

Tellurium  selenate,  2TeO2,  SeO3. 

As  sulphate.  (Metzner,  A.  ch.  1898,  (7) 
15.  203.) 

Thallous  selenate,  Tl2SeO4. 

SI.  sol.  in  cold,  much  more  in  hot  H2O. 
Insol.  in  alcohol  and  ether.  (Kuhlmann.) 

100  g.  H2O  dissolve  2.13  g.  at  9.3;  2.4  g. 
at  12°;  10.86  g.  at  100°.  (Tutton,  Proc. 
Roy.  Soc.  1907,  79.  A,  351.) 

2.8  g.  are  sol.  in  100  g.  H2O  at  20°;  8.5  g. 
at  80°.  (Glauser,  Z.  anorg.  1910,  66.  437.) 


Thallous     hydrogen 

3H2O. 
(Oettinger.) 


selenate,     HTlSeO4 


Thallous  zinc  selenate,   Tl2SeO4,  ZnSeO4+ 

6H2O. 

Easily  sol.  in  H2O,  but  less  than  the  cor- 
responding sulphate.  (Werther.  Bull.  Soc. 
1866.  60.) 

Thorium  selenate,  Th(SeO4)4+9H2O. 

100  pts.  H2O  dissolve  0.498  pt.  Th(SeO4)4 
at  0°,  and  1.972  pts.  at  100°.  (Cleve.) 


SELENITE,   CADMIUM 


791 


Tin  (stannic)   selenate,  basic,  SnO(SeO4)  + 

H2O. 

Deliquescent.  Sol.  in  H2O.  (Ditte,  C.  R. 
104.  231.) 

Uranyl   selenate,    (UO2)SeO4,   H2SeO4+ 
18H2O. 

Very  deliquescent. 

2(UO2)SeO4,  H2SeO4  +  12H2O.  Efflores- 
cent. Sol.  in  H2O.  (Sendtner,  A.  196.  325.) 

Ytterbium  selenate,  Yb2(SeO4)3. 

Anhydrous. 

+  15H2O  (?),  +8H2O.  Ppt.  (Cleve,  Z. 
anorg.  1902,  32.  145.) 

Yttrium  selenate,  Y2(SeO4)3. 

Anhydrous.  Sol.  in  H2O  with  hissing  and 
evolution  of  heat.  (Popp.) 

+8H2O.    Easily  sol.  in  H2O.    (Cleve.) 

-j-9H2O.    Efflorescent. 

Zinc  selenate,  ZnSeO4+5H2O. 
Sol.  in  H2O.    (Topsoe.) 
+6H2O.    Sol.  in  H2O.    (Topsoe.) 
+7H2O.    Sol.  inH2O. 

Selenious  acid,  H2SeO3. 

Deliquescent  in  moist,  efflorescent  in  dry 
air.  Very  sol.  in  cold,  and  in  nearly  every 
proportion  in  hot  H2O.  Easily  sol.  in  alcohol. 
(Berzelius.) 

Sp.  gr.  of  H2SeO3  and  of  H2SeO3+Aq  at  t°. 
Two  series  of  experiments. 


t° 

fc 

5P-  gr. 
att° 

H2SeO3+Aq  (A) 
1  vol.  A  +0.5  vol.  H2O 
'  +  1.0 
'  +  1.5 
'+2.0 
'+2.5 
'+3.0 

18.0 
18.0 
17.7 
16.6 
14.0 
17.0 
19.2 

] 

L.4386 
t.3179 
L.2337 
1.2045 
L1984 
L.1712 
L1600 

H2Se03+Aq  (B) 
1  vol.  B+0.5  vol.  H2O 
'  +  1.0 
'  +  1.5 
'+2.0 
'+2.5 
'+3.0 

15.8 
16.5 
13.0 
14.2 
17.0 
16.5 
14.2 

.4698 
.3191 
.2515 
.2074 
.1992 
.1793 
.1678 

(de  Coninck,  C.  C.  1906,  I.  1693.) 
See  also  Selenium  dioxide. 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  830.) 

Selenites. 

Alkali  selenites  are  sol.  in  H2O.  The  other 
neutral  selenites  are  insol.  in  H2O,  but  sol.  in 
HNO3+Aq,  Pb,  and  Ag  salts'  slowly.  The 


neutral  salts  are  insol.  in  HCl+Aq.    The  acid 
salts  of  the  heavy  metals  are  sol.  in  H2O.   • 

Aluminum  selenite,  basic,  4A12O3,  9SeO2+ 

36H20. 
Precipitate.    (Nilson,  Upsala,  1876.) 

Aluminum  selenite,  Al2(SeO3)3. 

Precipitate.    (Berzelius.) 

+7H2O.  SI.  sol.  in  H2O.  (Nilson.)  Sol. 
in  H2SeO3+Aq. 

+3H2O.  Insol.  in  H2O;  sol.  in  acids. 
(Boutzoureano,  A.  ch.  (6)  17.  289.) 

Aluminum  selenite,  acid,  A12O3,  4SeO2  + 
3H2O. 

( Boutzoureano . ) 

2A12O3,  9SeO2  +  12H2O.  Sol.  in  H2O.  (Nil- 
son.) 

A12O3,  6SeO2.  Very  sol.  in  H2O.  (Ber- 
zelius.) 

+5H2O.    (Nilson.) 

+2H2O.    (Boutzoureano.) 

Ammonium  selenite,  (NH4)2SeO3. 

Deliquescent.    Very  sol.  in  H2O. 

Precipitated  from  aqueous  solution  by  al- 
cohol. Insol.  in  ether.  (Muspratt,  A.  70. 
275.) 

Ammonium  hydrogen  selenite,  NH4HSeO3. 
Not  deliquescent.  Sol.  in  H2O.    (Berzelius.) 

Ammonium  /rihydrogen  selenite, 

NH4H3(Se03)2. 
Deliquescent.    (Berzelius.) 

Ammonium  vanadium  selenite. 
See  Vanadioselenite,  ammonium. 

Ammonium    uranyl    selenite,     (NH4)2SeO8, 

(UO2)SeO3. 
Completely  insol.  in  H2O.    (Sendtner.) 

Antimony  selenite,  Sb2(SeO3)3,  SeO2. 
(Nilson,  Bull.  Soc.  (2)  23.  494.) 

Barium  selenite,  BaSeO8. 

81.  sol.  in  H2O.  Sol.  in  H2SeO3+Aq.  So 
in  acids.  (Nilson.) 

+H2O.     (Nilson.) 

Baiium  pyroselenite,  BaSe2O6. 

Very  si.  sol.  in  cold,  more  in  warm  HjO. 
(Berzelius.) 

Bismuth  selenite,  Bi2(SeO3)3,  H2SeO3. 
(Nilson.) 
Bi2(SeO3)3.     (Nilson.) 

Cadmium  selenite,  CdSeOs. 

Insol.  in  H2O.  Sol.  in  H2SeO3+Aq.  (Mus- 
pratt, Chem.  Soc.  2.  65.) 


792 


SELENITE,   CADMIUM,   AMMONIA 


2CdO,  3SeO2+H2O.     Insol.  in  H2O;  sol. 
in-  acids.    (Boutzoureano.) 

Insol.  in  H2O;  sol.  in  dil.  acids. 


(Boutzoureano.) 

Cadmium  selenite  ammonia,  CdSeO3,  NH3. 
Insol.  in  cold  or  hot  H2O.    (Boutzoureano, 
A.  ch.  (6)  17.  289.) 

Calcium  selenite,  CaSeO3+4/3H2O. 

Very  si.  sol.  in  H2O.  (Berzelius.)  More 
sol.  in  H2SeO3-f  Aq. 

+2H2O.    (Nilson.) 

Calcium  hydrogen  selenite,  CaH2(Se03)2  + 
H2O. 

Quite  sol.  in  H2O.     (Nilson.) 

Ca2H2Se4On.  Easily  sol.  in  H2O.  (Nil- 
son.) 

Cerous    selenite,    basic,    2Ce203,    5SeO2  + 

30H2O. 
Precipitate.     (Nilson.) 

Cerous  selenite,  Ce2(SeO3)3+3H2O. 

Insol.  in  H2O.  Sol.  in  much  selenious  acid. 
(Jolin.) 

+  12H2O.    (Nilson.) 

Cerous  selenite,  acid,  Ce2O3,  4SeO2+5,  or  6 

H20. 

\"  Insol.  in  H2O,  but  sol.  in  selenious,  and 
other  acids.     (Jolin.) 

Ce2O3,  6SeO2+5H2O.  Not  decomp.  by 
H2O.  (Nilson.) 

Ceric  selenite,  Ce(SeO3)2. 

Insol.  in  H2O. 

SI.  sol.  in  cone.  HNO3.    Sol.  in  dil.  acids. 

Sol.  in  H2O2+Aq.  (Barbieri,  B.  1910,  43. 
2215.) 

Chromium  selenite,  basic,  4Cr2O3,  9SeO2  + 

64H2O. 
Precipitate.     (Nilson.) 

Chromic  selenite,  Cr2(SeO3)2+3H2O. 

(Boutzoureano.) 

+15H2O.    (Nilson.) 

Very  si.  sol.  or  insol.  in  H2O;  si.  sol.  in 
H2SeO3+Aq;  sol.  in  hot  cone.  HCl+Aq. 
(Taquet,  C.  R.  96.  107.) 

Chromic  selenite,  acid,  Cr2O3,  4SeO2  +  13H2O. 

Slowly  sol.  in  HCl+Aq.  Insol.  in  H2O. 
rfNilson.) 

CraO8,  5SeO2+9H2O.  Insol.  in  H2O. 
((Nilson.) 

Chromic  ^selenite. 

Insol.  in  H2O;  sol.  in  acids.  (Taquet,  C. 
H.  97.  1435.) 


Cobaltous  selenite,  CoSeO3. 
Insol.  in  H2O.     (Berzelius.) 

Insol.   in  H2O;   sol.   in  acids. 


(Boutzoureano,  A.  ch.  (6)  17.  289.) 

Cobaltous  hydrogen  selenite,   CoH2(SeO3)2. 

Sol.  in  H20.    (Berzelius.) 

+2H2O.  Sol.  in  H2O  with  decomp. 
(Boutzoureano.) 

Cuprous  selenite. 

Insol.    in    H2O.      Sol.    in    NH4OH+Aq. 

(Berzelius.) 

Cupric  selenite,  basic,  2CuO,  SeO2. 

Insol.    in    H2O;    sol.    in    NH4OH+Aq. 

(Boutzoureano.) 
Sol.  in  acids. 

Cupric  selenite,  CuSeO3  +  ^H2O. 

Insol.  in  H2O  or  H2SeO3+Aq.    (Berzelius.) 

+H2O,  and  2H2O.     (Boutzoureano.) 

-f  2H2O.    Min.  Chalcomenite.    Insol.  in  H2O 

or  H2SeO3+Aq.    (Friedel  and  Sarasin,  Zeit. 

Kryst.  1881,  6.  300.) 

Cupric  selenite,  acid,   CuO,  2SeO2+H2O  = 

CuH2(SeO3)3. 

Insol.  in  H2O.    Sol.  in  acids.     (Nilson.) 
+2H2O.    As  above.    (Boutzoureano.) 
k     +4H2O.     As  above.     (B.) 

Cupric   selenite   ammonia,   CuSeO3,   NH8  + 

H20. 

Decomp.  by  H2O.  (Boutzoureano,  A.  ch. 
(6)  17.  289.) 

Didymium  selenite,  basic,  3Di2O3,  8SeO2  + 
28H2O. 

Precipitate.     (Nilson.) 

+21H2O.  Insol.  in  H2O.  (Cleve,  Bull. 
Soc.  (2)  43.  363.) 

Didymium  selenite,  Di2(SeO3)3+6H2O. 
Precipitate.     (Smith.) 

Didymium    selenite,    acid,    Di2O3,    4SeO2  + 

5H2O. 

Precipitate.     (Cleve.) 

Composition  is  Di2(SeO3)34-6H2O.  (Smith.) 
+9H2O.     (Nilson.) 
2Di2O3,  9SeO2  +  18H2O.    (Nilson.) 

Erbium     selenite,     Er2(SeO3)3+5H2O,     and 

9H2O. 
Precipitate.     (Nilson.) 

Erbium  hydrogen   selenite,   Er2H2(SeO3)4  + 

4H20. 
Decomp.  by  hot  H2O. 


SELENITE,   MAGNESIUM  HYDROGEN 


793 


Gadolinium  hydrogen  selenite, 

Gd2(SeO3)3,  H2SeO3+6H2O. 
Ppt.      (Benedicks,    Z.    anorg.    1900,    22. 
413.) 

Glucinum  selenite,  basic,  5G1O,  2SeO2  + 
10H2O. 

Precipitate.  (Nilson.)  According  to  Atter- 
berg,  is  7G1O,  3SeO2  +  14H2O. 

2G1O,  SeO2+4H2O.  (Atterberg,  Bull.  Soc. 
(2)  19.  497.) 

3G1O,  2SeO2+6H2O.  Insol.  in  H2O. 
(Atterberg.) 

Glucinum  selenite,  GlSeO4+2H2O. 

Sol.  in  little  H2O,  decomp.  by  excess. 
(Nilson.) 

Glucinum  selenite,  acid. 

(a)  3G10,  5Se02+3H20;  (&)  G1O,  2SeO2 
+H2O;  (c)  3G1O,  7SeO2+5H2O;  (d)  G1O, 
3SeO2+2H2O.  All  are  very  si.  sol.  in  cold 
or  warm  HaO.  a,  b,  and  c  are  sol.  in  warm 
H2O  containing  HC1;  d  is  sol.  only  in  boiling 
dil.  HCl+Aq.  (Nilson.) 

Indium  selenite,  basic,  In8Se9O3o+64H2O. 
(Nilson.) 

Indium  selenite,  In2(SO3)3+6H2O. 
SI.  sol.  in  H2O.     (Nilson.) 

Indium     hydrogen     selenite,     In2(SeO3)3, 
3H2SeO3+4H2O. 

Sol.  in  H2O.     (Nilson.) 

2In2(SeO3)3,  3H2SeO3+12H2O.  Sol.  in 
H2O.  .(Nilson.) 

Iron  (ferrous)  selenite. 

Ppt.  Sol.  in  HCl+Aq  with  partial  separa- 
tion of  Se.  (Berzelius.) 

Iron  (ferrous)  hydrogen  selenite. 
SI.  sol.  in  H2O.    (Berzelius.) 

Iron  (ferric)  selenite,  basic,  2Fe2O3,  3SeO2  + 
*H20. 

Insol.  in  H20.    (Berzelius.) 

Fe2O3,  2SeO2.  Insol.  in  H2O,  easily  sol.  in 
acids.  (Boutzoureano,  A.  ch.  (6)  17.  289.) 

3Fe2O3,  8SeO2+28H2O.  Insol.  in  H2O. 
(NiLson.) 

Iron   (ferric)   selenite,  Fe2(SeO3)3+4H2O. 

Insol.  in  H2O.  (Muspratt,  Chem.  Soc.  2. 
52.) 

-fH2O.  Insol.  in  H2O.  (Boutzoureano, 
A.  ch.  (6)  17.  289.) 

+3H2O.     Insol.  in  H2O.     (B.) 

+  10H2O.    Insol.  in  H2O.    (B.) 


Iron  (ferric)  selenite,  acid,  Fe2O3,  6SeO2  + 
rcH2O. 

Insol.  in  H2O.  Sol.  in  HCl+Aq.  (Ber- 
zelius.) 

+2H2O.  (Boutzoureano,  A.  ch.  (6)  17. 
289.) 

Fe2O3,  4SeO2+H2O.  Insol.  in  H2O;  sol.  in 
acids.  (Boutzoureano.) 

Lanthanum  selenite,  basic,  3La2O3,  8SeO2  + 

28H20. 
Precipitate.    (Nilson.) 

Lanthanum  selenite,   La2(SeO3)3+9H2O,   or 

12H2O. 
Insol.  in  H2O.    (Nilson.) 

Lanthanum    selenite,    acid,    La2H4(SeO3)5  + 

4H2O. 
(Nilson.) 
La2H6(SeO3)6+2H2O.  (Cleve.) 

Lead  selenite,  PbSeO3. 

Scarcely  sol.  in  H2O,  even  when  it  contains 
H2SeO3.  SI.  sol.  in  HNO3+Aq.  (Berzelius.) 

Lithium  selenite,  Li2SeO3+H2O. 

Difficultly  sol.  in  H2O.  (Nilson,  Bull.  Soc. 
(2)  21.  253.) 

Lithium  hydrogen  selenite,  LiHSO3. 
Very  sol.  in  H2O.    (Nilson.) 

Lithium  /nhydrogen  selenite,  LiH3(SeO3)2. 
Not  deliquescent.    Sol.  in  H2O.    (Nilson.) 

Lithium  vanadium  selenite. 
See  Vanadioselenite,  lithium. 

Magnesium  selenite,  MgSeO3+2H2O. 

Insol.  in  H2O;  sol.  in  dil.  acids,  especially 
if  warm,  also  in  H2SeO3+Aq.  (Boutzour- 
eano, A.  ch.  (6)  18.  302.) 

+3H2O.  Very  si.  sol.  in  hot  H2O.  (Ber- 
zelius.) 

+6H2O.  As  the  2H2O  salt.  (Boutzour- 
eano.) 

+7H2O.  SI.  sol.  in  H2O.  Easily  sol.  in 
acetic,  and  mineral  acids.  (Hilger,  Z.  anal. 
13.  132.) 

Magnesium  hydrogen  selenite,  MgH2(SeO3)2 
+3H2O. 

Very  deliquescent.  Easily  sol.  in  H2O. 
(Nilson.) 

Insol.  in  alcohol.    (Muspratt.) 

MgO,  2SeO2.  Insol.  in  H2O;  sol.  in  acids. 
(Boutzoureano.) 

Magnesium  ^rahydrogen  selenite, 

MgH4(SeO3)3,  and  +3H2O. 
Sol.  in  H2O.     (Nilson.) 


794 


SELENITE,   MANGANOUS 


Manganous  selenite,  MnSeO3+H2O. 
Precipitate.     (Nilson.) 
+2H2O.    Insol.  in  H2O.     (Berzelius.) 
Sol.  in  cold  HCl+Aq.    (Muspratt.) 
+  3^H2O.    Insol.  in  H2O;  sol.  in  dil.  acids. 

(Boutzoureano.) 

Manganous  selenite,  acid,  MnSe2O5. 
Sol.  in  H2O.    (Berzelius;  Nilson.) 
MnO,   2SeO2+H2O  =  MnH2(SeO3)2. 

(Boutzoureano,  A.  ch.  (6)  17.  289.) 

+5H2O.    Decomp.  by  H2O  to  MnSeO3. 

(Boutzoureano.) 

Manganic  selenite,  basic,  Mn2O3,  2SeO2. 

Insol.  in  H2O,  cold  H2SO4,  or  HNO3+Aq; 
insol.  in  hot  dil.  H2SO4  or  HNO3+Aq. 
(Laugier,  C.  R.  104.  1508.) 

Sol.  in  warm  HCl+Aq  with  decomp. 

Manganic  selenite,  Mn2(SeO3)3+5H2O. 

(Laugier.) 
Manganic  selenite,  acid,  Mn2O3,  4SeO2. 

Insol.  in  H2O,  cold  H2SO4,  and  HNO3+Aq. 
Insol.  in  dil.  hot  H2SO4,  and  HNO3 + Aq.  Sol. 
in  cold  HCl+Aq;  and  in  H2SO3+Aq  with 
separation  of  Se.  (Laugier,  C.  R.  104.  1508.) 

Mercurous  selenite,  basic,  3Hg2O,  2SeO2  + 
5H20. 

(Boutzoureano.) 
Mercurous  selenite,  Hg2SeO3. 

Insol.  in  H2O  or  H2SeO3+Aq.  Sol.  in  hot 
HNO3+Aq.  (Kohler,  Pogg.  89.  146.) 

SI.  sol.  in  HCl+Aq,  and  KOH+Aq.    (Ber- 
zelius.) 
Mercurous  selenite,  acid,  3Hg2O,  4SeO2. 

Insol.  in  H2O  or  H2SeO3+Aq.    SI.  sol.  in 
boiling  HNO3+Aq.     (Kohler.) 
Mercuric  selenite,  basic,  7HgO,  4SeO2. 

Insol.   in   H2O.     SI.   sol.   in   HNO3+Aq. 
Easily  sol.  in  HCl+Aq.     (Kohler,  Pogg.  89. 
146.) 
Mercuric  selenite,  HgSeO3. 

Insol.  in  H2O.  (Berzelius.)  Nearly  insol. 
in  HNOs+Aq.  Sol.  in  K2SeO3+Aq.  (Di- 
vers, Chem.  Soc.  48.  585.) 

Insol.  in  dil.  HNO3+Aq;  sol.  in  HCl+Aq. 
(Rosenheim  and  Pritze,  Z.  anorg.  1909,-  63. 
278.) 

Solubility  in  Na2SeO,+Aq  at  25°. 


Na2SeO3+Aq 
Normality 

%  HgSeOs 

2.0 
1.0 
0.5 
0.25 
0.125 
0.0625 

2.73 
1.39 
0.70 
0.53 
0.32 
0.18 

(Rosenheim  and  Pritze,  Z.  anorg.  1909,  63. 
281.) 


HgSeO3,  H2SeO3.    Fasily  sol.  in  H2O;  very 
si.  sol.  in  alcohol.    (Berzelius.) 
See  also  selenium  dioxide. 

Mercuric  sodium  selenite,  HgSeO3,  Na2SeO3. 
Decomp.  by  H2O  and  alkalies  with  pptn. 
of    HgSeO3.        (Rosenheim    and    Pritze,    Z. 
anorg.  1909,  63.  279.) 

Mercuric  selenite  sodium  chloride, 

HgSeO3,  NaCl+2H2O. 
Decomp.  by  H2O.    (Rosenheim  and  Pritze, 
Z.  anorg.  1909,  63.  280.) 

Nickel  selenite,  NiSeO3+H2O. 

Insol.  in  H2O;  sol.  in  H2SeO3+Aq.  (Mus- 
pratt, Chem.  Soc.  2.  52.) 

+  34H2O.  Insol.  in  H2O.  (Boutzoureano, 
A.  ch.  (6)  17.  28.) 

Nickel  selenite,  acid. 
Sol.  in  H2O.    (Berzelius.) 

Potassium  selenite,  K2SeO3+H2O. 

Very  deliquescent.  Sol.  in  nearly  all  pro- 
portions in  H2O.  Insol.  in  alcohol,  which 
separates  it  as  oil  from  aqueous  solution. 
(Muspratt,  Chem.  Soc.  2.  52.) 

Potassium  hydrogen  selenite,  KHSeO3. 

Very  deliquescent.  Very  si.  sol.  in  alcohol. 
(Muspratt,  Chem.  Soc.  2.  52.) 

Potassium  ^nhydrogen  selenite,  KH3(SeO3)2. 

Very  deliquescent.  Pptd.  from  H2O  by 
alcohol.  (Muspratt.) 

Not  deliquescent.     (Nilson.) 

Potassium  hydrogen  pyroselenite,  KHSe2O5 

+H20. 
(Muthmann,  B.  1893,  26.  1015.) 

Potassium   uranyl    selenite,    K2SeO3, 

(UO2)SeO3. 
Absolutely  insol.  in  H2O.     (Sendtner.) 

Praseodymium  hydrogen  selenite, 

Pr2(SeO3)3,  H2SeO3+3H2O. 
Sol.    in    H2O.      (von    Scheele,    Z.    anorg. 
1898,  18.  362.) 

Samarium  selenite,  basic,  3Sm2O3,  8SeO2  + 

7H20. 
Precipitate.     (Cleve.) 

Samarium   selenite,   acid,    Sm2O3,    4SeO2  + 

5H20. 
Precipitate.     (Cleve.) 

Scandium  selenite,  Sc2(SeO3)3+H2O. 
Insol.  precipitate. 


SELENITE,  ZIRCONIUM,  BASIC 


795 


Scandium    hydrogen     selenite,     Sc2(SeO3)3 

3H2SeO3. 

Insol.  in  H2O.  Not  attacked  by  cold  dil 
acids,  but  easily  if  warmed. 

Silver  selenite,  Ag2SeO3. 

Very  si.  sol.  in  cold,  somewhat  more  sol.  in 
hot  H2O.  Easily  sol.  in  hot  HNO3+Aq, 
from  which  it  is  precipitated  by  H2O 
(Berzelius.) 

Insol.  in  K2SeO3+Aq;  si.  sol.  in  dil  HNO3  + 
Aq.  (Divers,  Chem.  Soc.  49.  585.) 

Silver  selenite  ammonia,  Ag2SeO3,  NH8. 

Insol.  in  boiling  H2O.  (Boutzoureano,  A 
ch.  (6)  17.  289.) 

Sodium  selenite,  Na2SeO3. 

Very  sol.  in  H2O.  Insol.  in  alcohol.  (Ber- 
zelius.) 

+5H20. 

Sodium  selenite,  acid,  NaHSeO3. 

Permanent.    Sol.  in  H2O. 

Na4Se3O8.  Sol.  in  H2O.  (Sacc,  A.  ch.  (3) 
21.  119.) 

NaH3(SeO3)2.  Not  deliquescent.  Sol.  in 
H20. 

Sodium  vanadium  selenite. 
See  Vanadioselenite,  sodium. 

Strontium  selenite,  SrSeO3+7H2O. 

Precipitate.  Insol.  in  H2O.  Sol.  in  HNO3 
+Aq.  (Muspratt.) 

Strontium  hydrogen  selenite,  SrH2(SeO3)2. 
Easily  sol.  in  hot  or  cold  H2O.     (Nilson.) 
Nearly  insol.  in  hot  or  cold  H2O.     (Ber- 
zelius.) 

Thallous  selenite,  Tl2SeO3. 

Easily  sol.  in  H2O.  Insol.  in  alcohol  and 
ether.  (Kuhlmann,  Bull.  Soc.  (2)  1.  330.) 

Thallous  hydrogen  selenite,  TlHSeO3. 

More  sol.  in  F2O  than  the  above  comp. 
(Kuhlmann.) 

ThaJlic  selenite,  Tl2(SeO3)3. 

Insol.  in  H2O.    Sol.  in  dil.  HNO3. 

Easily  decomp.  by  HC1  and  H2SO4.  (Ma- 
rino, Z.  anorg.  1909,  62.  177.) 

Thorium  selenite,  Th(SeO3)2+H2O,  or  8H2O. 
Insol.   in   H2O;   easily   sol.   in   HCl+Aq. 
(Nilson.) 

Thorium    selenite,    acid,    2Th02}    7SeO2+ 

16H2O. 
ThO2,  5SeO2+8H2O.    (Nilson.) 


Tin  (stannic)  selenite. 

Insol.  in  H2O;  sol.  in  HCl+Aq,  from  which 
it  is  pptd.  by  H2O.  (Berzelius.) 

Uranic  selenite,  U2O3,  SeO2. 

Insol.  in  H2O.    (Boutzoureano.) 
+2H20.    (B.) 

Uranic  selenite,  acid,  2U2O3,  3SeO2+7H2O. 

Insol.  in  H2O.  (Boutzoureano,  A.  ch.  (6) 
17.  289.) 

Uranyl  selenite,  (UO2)SeO3+2H2O. 
Precipitate.     (Nilson.) 

Uranyl  selenite,  acid,  3UO3,  5SeO2+7H2O,  or 
9H2O. 

Insol.  in  H2O. 

UO3,     2SeO2+H2O  =  (UO3)H2(SeO3)2. 
Absolutely  insol.  in  H2O  and  H2SeO3+Aq. 
(Sendtner,  A.  195.  325.) 

Vanadium  selenite. 
See  Vanadioselenious  acid. 

Ytterbium  selenite,  Yb2(SeO3)3. 
Insol.  precipitate. 

Ytterbium  hydrogen  selenite,  Yb2H2(SeO3)4 

+4H2O. 
Insol.  in  H2O. 

Yttrium  selenite,  Y2(SeO3)3  +  12H2O. 

Insol.  in  H2O  or  H2SeO3+Aq.    (Berzelius.) 
Sol.inhotH2SeO3+Aq.    (Nilson.) 

Yttrium   hydrogen    selenite,   Y2H2(SeO3)4+ 

3H2O. 

SI.  sol.  in  H2O.  Easily  sol.  in  HC1  or 
HNO3+Aq.  (Cleve.) 

Zinc  selenite,  ZnSeO3. 

Insol.  in  H2O;  sol.  in  acids.  (Boutzoureano, 
A.  ch.  (6)  18.  289.) 

+2H2O.  Insol.  in  H2O.  Sol.  in  H2SeO3, 
or  HNO3+Aq.  (Muspratt,  Chem.  Soc.  2. 

Zinc  hydrogen  selenite,  ZnH2(SeO3)2. 
Easily  sol.  in  H2O.    (Berzelius.) 
+2H2O.     Sol.  in  cold  H2O.     (Boutzour- 
eano.) 

ZnO,  4SeO2+3H2O.     Easily  sol.  in  H2O 
(Wohler,  A.  63.  279.) 

Zinc  selenite  ammonia,  ZnSeO3,  NH3. 

Insol.  in  cold  or  hot  H2O.  (Boutzoureano. 
A.  ch.  (6)  17.  289.) 

Zirconium   selenite,   basic,   4ZrO2,    3SeO2  + 
18H2O. 

Precipitate.  SI.  sol.  in  HCl+Aq.  (Nil-. 
son.) 


796 


SELENITE,  ZIRCONIUM 


Zirconium  selenite,  Zr(SeO3)2. 

Absolutely  insol.  in  H2O;  difficultly  sol.  in 
boiling  HCl+Aq.  (Nilson.) 

+H2O.    (Nilson.)- 

Selenium,  Se. 

Insol.  in  H2O.  Schultz  (J.  pr.  (2)  32.  390) 
has  obtained  a  soluble  colloidal  modifica- 
tion which  can  be  isolated  by  dialysis. 

Insol.  in  HCl+Aq.  Decomp.  by  HNO3  + 
Aq.  Sol.  in  fuming  H2SO4.  (Schultz-Sellac, 
B.  4.  113.) 

1000  pts.  CS2  dissolve  1  pt.  cryst.  Se  at 
boiling-point  (46.6°),  and  0.16  pt.  at  0°  (Mit- 
scherlich,  J.  B.  1856,  314.)  Solubility  of  Se 
in  CS2  is  variable — 1  pt.  Se  is  sol.  in  1376- 
2464-3746  pts.  CS2  at  20°  (Rammelsberg,  B. 
7.  66,0).  Cryst.  Se,  which  is  sol.  in  CS2,  be- 
comes insol.  in  CS2  after  heating  to  110°,  but 
after  fusion  is  again  sol.  (Otto). 

Four  modifications. — •(!)  Amorphous  red; 
(2)  crystalline  red;  (3)  granular  gray;  (4) 
laminated.  1  and  2  are  sol.  in  CS2,  3  and  4  are 
insol.  in  CS2.  All  forms  are  sol.  in  SeCl2, 
from  which  crystallizes  a  black  modification, 
insol.  in  CS2.  CC14  with  trace  of  CS2  dis- 
solves red  Se  slightly,  black  Se  not  at  all. 
Se(C2H6)2  dissolves  all  modifications  in 
small  but  apparently  equal  quantities. 
(Rathke,  A.  152.  181.) 

According  to  Saunders  (J.  phys.  Chem. 
1900,  4.  428)  selenium  exists  in  three  modi- 
fications. 

1.  Liquid,  including  vitreous,  amorphous, 
and  colloidal  selenium. 

a.  Vitreous. 

Sol.  in  liquid  NH3  at  25°.  (Franklin,  Am. 
Ch.  J.  1898,  20.  820.) 

Insol.  in  liquid  NH3  between  — 30°  and 
+  10°.  Franklin's  results  are  due  to  impure 
selenium  and  not  completely  dry  NH3. 
(Hugot,  A.  Ch.  1900,  (7)  21.  5.) 

Almost  insol.  in  CS2.  (Schiitzenberger 
Chimie  ge"ne"rale  1.  438.) 

Action  of  light  increases  solubility  in  CS2. 
(Saunders,  J.  phys.  Chem.  1900,  4.  456.) 

Solubility  in  methylene  iodide  at  12°  is 
1.3  pts  in  100.  (Retgers,  Z.  anorg.  1893, 
3.  343.) 

Sol.  in  CSe2,  ethyl  selenide,  and  in  ethyl 
sulphide. 

Very  sol.  in  Se2Cl2.  (Rathke,  A.  1869,  162. 
181.) 

b.  Amorphous. 

Completely  sol.  in  CS2  at  ord.  temp,  if 
Se  has  not  been  heated.  If  heated  or  ex- 
tracted with  warm  CS2  it  becomes  partly 
insol.  (Peterson,  Z.  phys.  Chem.  1891,  81. 
612.) 

Passes  into  red  crystalline  form  in  solution 
in  CS2,  C6H6,  isobutyric  acid,  acetophenone, 
acetone,  CHC13,  thiophene,  toluene,  ben- 
zonitrile,  ethyl  acetate,  and  alcohol.  (Saun- 
ders, J.  phys.  Chem.  1900,  4.  463.) 

Solution  in    quinoline,     aniline,   pyridine, 


etc.,  cause  conversion  into  gray  metallic 
form. 

c.  Colloidal. 

Forms  colloidal  solution  with  H2O. 

A  colloidal  solution  of  Se  in  H2O  can  be 
obtained.  It  is  not  decomp.  by  boiling,  but 
is  decomp.  by  electrolytes  with  separation  of 
red  selenium.  (Gutbier,  Z.  anorg.  1902,  32. 
106.) 

2.  Red  crystalline. 
Sol.  in  CS2. 

3.  Gray,  crystalline  or  metallic. 

Sol.  in  selenium  chloride  and  other  solv- 
ents as  vitreous  Se.  (Rathke,  A.  1869,  152. 
181.) 

SI.  sol.  in  CS2,  toluene,  nitrobenzene, 
quinoline,.  aniline,  and  KOH.  Pptd.  from 
cone.  KOH+Aq.  in  long  needles  with  mpt. 
219°.  (Coste,  C.  R.  1909,  149.  674.) 

Sol.  in  many  organic  substances  at  high 
temp,  as  quinoline,  ethyl  benzoate,  aniline 
and  naphthaline.  (Saunders,  J.  phys.  Chem. 
1900,  4.  469.) 

Completely  insol.  in  CS2.  (Saunders,  J. 
phys.  Chem.  1900,  4.  474.) 


Solubility  of  the  two  modifications  of  gray 
crystalline  Se  in  CS2. 

100  cc.  boiling  CS2  dissolve  mg.  Se. 
I  II  in 


Mg.  Se 

Mg.  Se 

Mg.  Se 

3.2 

4.1 

2.7 

2.8 

4.0 

2.2 

3.6 

2.9 

1.9 

3.3 

2.8 

1.0 

2.2 

2.9 

2.0 

4.0 

I.  Se  heated  1  hr.  at  140°.    Modification  A. 

II.  Modification  A. 

III.  Se    heated     48     hrs.    at    190°-200°. 
Modification  B. 

(Marc,  Z.  anorg.  1907,  53.  302.) 

Se2Br2  dissolves  22%  Se.  (Schneider, 
Pogg.  128.  327.) 

Red  Se  is  sol.  in  (NH4)2SO3+Aq.  (Uels- 
mann,  A.  116.  122.) 

Sol.  in  alkalies  and  Mg  sulphites +Aq. 

365  pts.  K2SO3+Aq  dissolve  102  pts.  Se. 

360  pts.  MgSO3,  3H2O+Aq  dissolve  116 
pts.  Se. 

Insol.  in  BaSO3+Aq.  (Rathke  and  Zschie- 
sche,  J.  pr.  92.  145.) 

Sol.  in  KCN-f-Aq  with  formation  of 
KSeCN.  (Franklin,  Am.  Ch.  J.  1898,  20. 
830.) 

100  pts.  methylene  iodide  dissolve  1.3  pts. 
Se  at  12°.  (Retgers,  Z.  anorg.  3.  343.) 

Sol.  in  quinoline,  but  reacts  with  the  solvent 
with  evolution  of  H.  (Beckmann  and  Gabel, 
Z.  anorg.  1906,  61.  236.) 


SELENIUM  OXIDE 


797 


Selenium  monobromide,  Se2Br2. 

Insol.  in  H2O,  but  gradually  decomp. 
thereby.  Decomp.  by  absolute  alcohol  and 
benzene.  Sol.  in  C2H6I,  but  soon  decomposed. 
Miscible  with  CS2;  less  sol.  in  CHCls  and 
C2H5Br.  (Schneider,  Pogg.  128.  327.) 

Selenium  te^rabromide,  SeBn. 

Sol.  in  H2O  with  decomp.  Decomp.  by 
alcohol.  Sol.  in  HCl+Aq;  si.  sol.  in  CS2, 
CHC13,  and  C2H5Br.  (Schneider,  Pogg. 
129.  430.) 

Decomp.  by  C2H5I. 

Selenium  bromo^nchloride,  SeCl3Br. 

Insol.  in  CS2.  (Fvans  '  and  Ramsay, 
Chem.  Soc.  46.  62.) 

Selenium     ^mbromide      sulphur     ^noxide, 

SeBr4,  2SO3. 

Decomp.  by  H2O.  (Prandtl,  Z.  anorg. 
1909,  62.  242.) 

Selenium  ^nbromochloride,  SeClBr3. 
See  Selenium  chlorc^nbromide. 

Selenium  monochloride,  Se2Cl2. 

Gradually  decomp.  by  H2O.  Dissolves 
all  modifications  of  selenium  on  heating 
(Rathke,  A.  152.  181).  Insol.  in  cone.  H2SO4; 
easily  sol.  in  fuming  H2SO4.  Sol.  in  CHC13, 
C6H6,  CC14.  Gradually  decomp.  by  H2O, 
alcohol,  and  ether.  (Divers  and  Shimose", 
B.  17.  862.)  Sol.  in  CS2.  (Evans  and  Ram- 
say, Chem.  Soc.  46.  62.) 

Selenium  te^rachloride,  SeCl4. 

Deliquescent  on  moist  air.  Decomp.  with 
H2O.  (Berzelius,  A.  ch.  9.  225.)  Insol.  in 
CS2.  Easily  sol.  in  hot  POC13,  from  which 
it  crystallizes  on  cooling.  (Michaelis,  Zeit. 
Chem.  (2)  6.  460.)  Very  si.  sol.  in  CS2. 
(Evans  and  Ramsay,  Chem.  Soc.  45.  62.) 

Selenium  dichlorobromide,  SeCl2Br2. 
(Evans  and  Ramsay,  Chem.  Soc.  45.  62.) 

Selenium  chlorofribromide,  SeClBr3. 

Very  si.  sol.  in  CS2.    (Evans  and  Ramsay.) 

Selenium   ^nchlorobromide,   SeCl3Br. 
See  Selenium  bromo^nchloride. 

Selenium  fluoride. 

Sol.  in  cone.  HF+Aq.  Decomp.  immedi- 
ately by  H2O.  (Knox.) 

Selenium  wonoiodide,  Se2l2. 

Decomp.  by  H2O.  All  solvents  of  iodine 
dissolve  out  that  element.  (Schneider, 
Pogg.  129.  627.) 


Selenium  tefraiodide,  SeI4. 

Slowly  decomp.  by  much  H2O.  Iodine  is 
dissolved  out  by  all  solvents  of  that  element. 
(Schneider,  Pogg.  129.  627.) 

Selenium  nitride. 
See  Nitrogen  selenide. 

Selenium  monoxide,  SeO  (?). 
SI.  sol.  in  H2O.     (Berzelius.) 
Does  not  exist.     (Sacc.) 


sol.    in    H2O    and 
HC2H3O2.     (Hins- 


Selenium  dioxide,  SeO2. 

Deliquescent.  Easily 
alcohol.  Sol.  in  glacial 
berg,  A.  260.  40) 

Solubility  in  H2O  between  — 3°  and  +36° 
=  45.0+0.7692t,  (Etard,  C.  R.  1888,  106. 
742.) 

1  pt.  is  sol.  in  2.67  pts.  H2O  at  11.3.° 
]  pt.   "    "    "  2.60     "       "      "  14.° 
1  pt.   "    "    "  2.54     "       "      "  15.6.° 
(de  Coninck,  C.  R.  1906,  142.  571.) 

Sp.  gr.  of  SeO2+Aq  at  t°. 


t° 

%  SeO2 

Sp.  gr. 

15.1 

1 

0.9923 

15.3 

2 

.0068 

13.0 

3 

.0200 

13.0 

4 

.0302 

14.5 

5 

.0346 

14.8 

6 

.0402 

14.1 

7 

.0535 

15.0 

8 

.0571 

15.6 

9 

1.0719 

15.2 

10 

1.0743 

(de  Coninck,  C.  R.  1906,  142.  571.) 
See  also  Selenious  acid. 

1  pt.  SeO2  is  sol.  in  9.84  pts.  alcohol  (93°) 
at  14.° 

1  pt.  SeO2  is  sol.  in  15.0  pts.  methyl  alco- 
hol at  11.8°. 

1  pt.  SeO2  is  sol.  in  23.0  pts.  acetone  at 
15.3.° 

1  pt.  SeO2  is  sol.  in  90.0  pts.  acetic  acid 
at   12.9/ 
572.) 


(de  Coninck,   C.   R.    1906,    142. 


Traces  dissolve  in  acetic  anhydride.  Sol. 
in  phenyl  mercaptan.  (Hinsberg,  A.  1890, 
260.  40.) 

Insol.  in  pure  C6H6.  (Clausnizer,  A.  1879, 
196.  271.) 

See  Selenious  acid. 


Selenium  In'oxide,  SeO3. 

Not  obtained  in  a  pure  state, 
and  Macallan.) 

See  Selenic  acid. 


(Cameron 


798 


SELENIUM  OXIDE  HYDROBROMIC  ACID 


Selenium  dioxide  hydrobromic  acid,  SeO2, 
4HBr. 

Decomp.  at  55.°  (Ditte,  A.  ch.  (5)  10. 
82.) 

SeO5,  5HBr.  Decomp.  at  65.°  (Ditte, 
A.  ch.  (5)  10.  82.) 

Selenium  dioxide  hydrochloric  acid.  SeO2, 
2HC1. 

Decomp.  at  26°. 

SeO2,  4HC1.  Decomp.  at  0°.  Sol.  in  H2O 
without  evolution  of  gas.  (Ditte,  A.  ch.  (5) 
10.  82.) 

Selenium  dioxide  sulphur  /n'oxide,  SeO2, 
SO3. 

Decomp.  violently  by  H2O.  (Weber,  B. 
19.  3185.) 

Composition  may  be  (SeO)SO4  (?). 

Selenium  oxy-compounds. 
See  Selenyl  compounds. 

Selenium  diphosphide,  P2Se. 
See  Phosphorus  monoselenide. 

Selenium  ^raphosphide,  P4Se. 
See  Phosphorus  se/m'selenide. 

Selenium  monosulphide,  SeS. 

Insol.  in  H2O  and  ether.  Sol.  in  CS2. 
Decomp.  by  alcohol.  (Ditte,  C.  R.  73.  625, 
660.) 

Other  compounds  of  Se  and  S  are  probably 
mixtures  of  the  two  elements. 

Selenium  disulphide,  SeS2. 

Compound  of  this  formula  is  a  mixture  of 
SeS  and  S.  (Ditte,  C.  R.  73.  625,  660.) 

Selenium  sulphoxide,  SeSO3. 

Decomp.  by  H2O.  Sol.  in  fuming  H2SO4, 
cone.  H2SO4.  Sol.  in  H2SO4  of  1.806  sp.  gr. 
without  decomp.  (Weber,  Pogg.  166.  531.) 

Decomp.  by  H2O;  sol.  in  H2SO4.  (Divers 
and  Shimose",  B.  17.  858.) 

Seleniuretted  hydrogen,  H2Se. 
See  Hydrogen  selenide. 

Selenoarsenic  acid. 

Potassium  selenoarsenate,  KAsSe3+2H2O. 

Only  si.  sol.  in  cold  H2O;  sol.  in  warm  H2O 
with  decomp.;  more  stable  in  KOH+Aq. 
(Clever,  Z.  anorg.  1895,  10.  132.) 

Sodium  selenoarsenate,  Na3AsSe4+9H2O. 

Very  sol.  in  H2O;  very  unstable.  (Szar- 
vasy,  B.  1895,  28.  2658.) 


Selenoarsenious  acid. 

Sodium  selenoarsenite,  Na3AsSe3+9H2O. 

Moderately  sol.  in  H2O.  (Clever  and 
Muthmann,  Z.  anorg.  1895,  10.  139.) 

Selenobismuthous  acid. 

Potassium  wetoselenobismuthite,  Bi2Se3,  K2Se 

or  KBiSe2. 

Insol.  in  cold  dil.  HCl-f-Aa.  Sol.  on  warm- 
ing, with  evolution  of  H2Se.  (Hilger  and 
van  Scherpenberg,  Mitt.  Pharm.  II.  4.) 

Selenocyanhydric  acid,  HSeCN. 
Known  only  in  aqueous  solution. 

Ammonium    selenocyanide,    NH4SeCN. 
Very  deliquescent,  and  sol.  in  H2O. 

Barium ,  Ba(SeSCIS)2. 

Very  sol.  in  H2O. 

Lead ,  Pb(SeCN)2. 

SI.  sol.  in  cold,  sol.  with  si.  decomp.  in 
boiling  H2O.  Insol.  in  alcohol. 

Mercurous ,  Hg2(SeCN)2. 

Ppt. 

Mercuric ,  Hg(SeCN)2. 

SI.  sol.  in  cold  H2O.  Easily  sol.  in  MCN, 
MSCN,  or  MSeCN+Aq;  also  sol.  in  hot 
HgCl2+Aq.  (Cameron  and  Davy,  C.  N.  44. 
63.) 

Decomp.  by  hot  H2O.  (Rosenheim,  Z. 
anorg.  1909,  63.  276.) 


Mercuric    potassium  — — ,    Hg(SeCN)2, 

KSeCN. 

Easily  sol.  in  H2O.  SI.  sol.  in  cold  alcohol. 
(Cameron  and  Davy,  C.  N.  44.  63.) 

Mercuric  selenocyanide  chloride, 
Hg(SeCN)2,  HgCl2. 

Sol.  in  boiling  H2O  and  in  abs.  alcohol. 

Decomp.  by  long  boiling  with  H2O.  (Rosen- 
heim and  Pritze,  Z.  anorg.  1909,  63.  276.) 

Platinum  potassium (Potassium  platino- 

selenocyanide),  K2Pt(SeCN)6. 
Sol.  in  H2O  and  alcohol.     (Clarke,  B.  11. 
1325.) 

Potassium  ,  KSeCN. 

Very  deliquescent,  and  sol.  in  H2O  with 
absorption  of  heat.  More  sol.  in  H2O  than 
KSCN.  Sol.  in  alcohol. 

Potassium mercuric  bromide,  KSeCN, 

HgBr2. 

SI.  sol.  in  cold,  more  easily  in  hot  H2O  or 
alcohol.  (Cameron  and  Davy,  C.  N.  44.  63.) 


SELENOSULPHARSENATE,  POTASSIUM 


799 


Potassium  selenocyanide  mercuric  chloride, 

KSeCN,HgCl2. 
As  the  bromide. 

Potassium   — — •  mercuric   iodide.    KSeCN, 

HgI2. 

SI.  sol.  in  cold,  easily  in  hot  H2O  or  alcohol 
(Cameron  and  Davy.) 

Potassium  mercuric   sulphocyanide. 

KSeCN,  Hg(SCN)2. 

SI.  sol.  in  cold,  much  more  in  hot  H2O  or 
alcohol.  Somewhat  sol.  in  ether.  (Cameron 
and  Davy.) 

Silver ,  AgSeCN. 

Insol.  in  H2O.  Almost  insol.  in  NH4OH  + 
Aq  or  cold  dil.  acids.  Quickly  decomp.  by 
hot  cone,  acids. 

Sodium -,  NaSeCN. 

Very  sol.  in  H2O. 

Selenomolybdic  acid. 

Potassium    selenomolybdate,    5K2O,    6SeO2, 

17MoO3. 

Readily  sol.  in  H2O  without  decomp. 
(Gibbs,  Am.  Ch.  J.  1895,  17.  177.) 

Selenopentathionic  acid. 

Sodium  selenopentatbionate,  Na2S4SeO6. 

A  dil.  solution  may  be  boiled  for  some  time 
without  change.  (Norris  and  Fay,  Am.  Ch. 
J.  1900,  23.  121.) 

Selenophosphoric  acid. 

Ammonium  selenophosphate, 

2(NH4)2O,  P2O5,  2SeO3+3H2O. 
Sol.  in  H2O  with  decomp.     (Weinland,  B. 
1903,  36.  1402.) 

Potassium  selenophosphate, 
2K2O,  P2O5,  2SeOs+3H2O. 

Sol.  in  H2O  with  decomp. 

3.5K2O,  P2O6,  5SeO3+5.5H2O.  Easily 
sol.  in  H2O.  (Weinland.) 

Rubidium  selenophosphate, 

2Rb2O,  P2O5,  2SeO3+3H2O. 
Sol.  in  H2O  with  decom.    (Weinland.) 

!Tnselenophosphorous  acid. 

Potassium  ^selenophosphite, 

K2HPSe3+2^H2O. 

Decomp.  by  moist  air  and  dil.  acids;  sol. 
in  cone.  KOH+Aq.;  si.  sol.  in  cold,  easily  sol. 
in  hot  H2O.  (Muthmann,  Z.  anorg.  1897, 
13.  198.) 


Selenosamic  acid,  HSeO2NH2. 

Known  only  in  its  salts. 

Ammonium  selenosamate,  (NH4)SeO2NH2. 

Deliquescent.  Decomp.  slowly  by  H2O 
into  (NH4)2SeO3. 

1  pt.  is  sol.  in  116  pts.  cold  alcoholic  am- 
monia at  12°.  More  sol.  in  hot  alcoholic 
ammonia.  SI.  attacked  by  cold  HC1  or  HNO3. 
(Cameron  and  Macallan,  C.  N.  1888,  67.  163.) 

Ammonium  hydrogen  selenosamate, 

NH4H(SeO2NH2)2. 

Deliquescent.  Sol.  in  14  pts.  alcohol  at 
14°.  (Cameron  and  Macallan,  Proc.  Roy. 
Soc.  44.  112.) 

Selenostannic  acid. 

Ammonium  selenostannate,  3SnSe2,  (NH4)2Se 

+3H2O. 
Sol.  in  H2O.    (Ditte,  C.  R.  95.  641.) 

Platinum  potassium ,  K2Se,  3PtSe,  SnSe2. 

Insol.  in  hot  or  cold  H2O,  NH4OH,  or 
KOH+Aq.  Not  attacked  by  hot  HCl+Aq. 
(Schneider,  J.  pr.  (2)  44.  507.) 

Platinum  sodium ,  Na2Se,  3PtSe,  SnSe2. 

Properties  as  the  corresponding  K  salt. 
(Schneider.) 

Potassium—,  K2SnSe3+3H2O. 

Easily  sol.  in  H2O.    (Ditte,  C.  R.  95.  441.) 

Selenosulphantimonic  acid. 

Sodium  selenosulphantimonate,  Na3SbSeS3  + 

9H2O. 

Sol.  in  H2O.    (Hofacker,  A.  107.  6.) 
Na3SbS1.5Se2.5+9H2O.     Somewhat  sol.  in 

H2O.    (Pouget,  A.  ch.  1899,  (7)  18.  564.) 

Selenosulphantimonous  acid. 

Potassium  selenosulphantimonite, 

Sb4S5Se6K10+4H2O. 

Sol.  in  H2O.  (Pouget,  A.  ch.  1899,  (7) 
18.  563.) 

Sodium  selenosulphantimonite,  Na3SbSi.6Sei.5 

+9H20. 

Sol.  in  H2O.  (Pouget,  A.  ch.  1899,  (7)  18. 
564.) 

Selenosulpharsenic  acid. 

Potassium  selenosulpharsenate,  3K2S,  As2Ses 

+12H20. 

Very  unstable  in  the  air.  Very  sol.  in  H2O. 
Fairly"  stable  in  aqueous  solution.  Decomp. 
by  acids.  (Clever,  Z.  anorg.  1895,  10.  134.) 


800 


SELENOSULPHARSENATE,  SODIUM 


Sodium    selenosulpharsenate.    Na3AsS3Se+ 
8H20. 

Decomp.  by  acids;  stable  in  dry  air. 
(Messinger,  B.  1897,  30.  801.) 

3Na2S,  As2Se8  +  18H2O.  Quite  sol.  in  H2O; 
quite  stable  in  air.  (Clever.  Z.  anorg.  1895, 
10.  140.) 


NaeAs2S6Ses 


SI.  sol.  in  H2O;  de- 


comp.  by  acids.     (Messinger,  B.   1897.  30. 


p 

.) 


803 

Stable  in  dry  air; 
easily  sol.  in  H2O;  decomp.  by  acids.  (Mes- 
singer, B.  1897,  30.  800.) 

Na3AsS2Se2+9H2O.  Decomp.  in  aq.  solu- 
tion by  dil.  acids.  (Messinger,  B.  1897,  30. 
802.) 

Na3AsSSe3+9H2O.  Sol.  in  H2O;  decomp. 
by  aq.  acids;  hydroscopic.  (Messinger.)' 

Selenosulphophosphorous  acid. 

Potassium      selenosulphophosphite,      2K2S, 
P2Se3+5H2O. 

Sol.  in  H2O;  decomp.  by  acids.  (Muth- 
mann,  Z.  anorg.  1897,  13.  198.) 

Selenosulphostannic  acid. 

Ammonium  selenosulphostannate,   (NH4)2S, 

3SnSe2+3H2O. 

Easily  decomp.  (Ditte,  C.  R.  1882,  95. 
643.) 

Potassium  —  —  ,  K2SnSe2S+3H2O. 

Very  easily  sol.  in  H2O.  (Ditte,  C.  R.  95. 
641.)  " 

Sodium  --  ,  Na2SnSe2S+3H2O. 
Sol.  in  H2O.    (Ditte,  C.  R.  96.  641.) 

Selenosulphoxyarsenic  acid. 

Sodium  selenosulphoxyarsenate,  Na3AsO2SSe 
+  10H2O. 

Easily  sol.  in  H2O  but  solution  rapidly 
decomp.  (Messinger,  B.  1897,  30.  798.) 

Na6As2S2SeO5+24H2O.     Sol.  in  H2O. 
(Messinger.) 

Na6As2SeS3O4+20H2O.  Stable  in  dry  air. 
SI.  sol.  in  H2O;  decomp.  by  dil.  acids.  (Mes- 
singer.) 

Na«As2S3Se2O3+20H2O.  Ppt.  (Messin- 
ger.) 

Na9As3S2Se2O8+36H2O.  Decomp.  by  aq. 
acids;  sol.  in  H2O;  quite  stable.  (Messinger.) 

Selenosulphur  dioxide,  SeSO3. 
See  Selenium  sulphoxide. 

Selenosulphuric  acid,  H2SeSO3.     • 
Known  only  in  its  salts. 


Potassium  selenosulphate,  K2SeSO3+zH2O. 

Deliquescent  in  moist  air;  decomp.  by  H2O. 
(Rathke,  J.  pr.  95.  1.) 

Selenotrithionic  acid,  H2S2SeO6. 

Known  only  in  solution,  which  is  stable  in 
dark.  (Schulze,  J.  pr.  (2)  32.  390.) 

Barium  selenotrithionate. 
Sol.  in  H2O.    (Rathke.) 

Potassium ,  K2SeS2O6. 

Sol.  in  H2O  with  gradual  decomp.  (Rathke 
J.  pr.  95.  8;  97.  56.) 

IH'selenotrithionic  acid,  H2SSe2O6. 
Exceedingly  unstable.    (Schulze.) 

Selenovanadic  acid. 

Lithium  selenovanadate,  4Li2O,  6V2Os,  5SeO2 

+30H2O. 

Very  sol.  in  H2O.  (Prandtl  and  Lustig,  Z. 
anorg.~  1907,  63.  401.) 

Potassium  selenovanadate,  2K2O,  3V2C>5, 
12SeO2  +  12H2O. 

(Prandtl  and  Lustig.) 

3K2O,  5V2O5,  16SeO2+40H2O.  (Prandtl 
and  Lustig.) 

4K2O,  6V2O5,  21SeO2+37H2O.  (Prandtl 
and  Lustig.) 

5K2O,  10V2O5,  26SeO2+43H2O.  (Prandtl 
and  Lustig.) 

Sodium  selenovanadate,  4Na2O,  6V2O5,  5SeO2 
+20H2O. 

Very  sol.  in  H2O.  Solution  decomp.  grad- 
ually. (Prandtl  and  Lustig.) 

2Na2O,  7V2O6,  10SeO2  +  13H2O.  (Prandtl 
and  Lustig.) 

2Na2O,  7V2O6,  12SeO2+45H2O,  and 
+90H2O.  (Prandtl  and  Lustig.) 

Selenoxyarsenic  acid. 

Ammonium   selenoxyarsenate,   2(NH4)2O, 

2SeO3,  As2O6+3H2O. 

Sol.  in  H2O  with  decomp.  (Weinland,  B. 
1903,  36.  1403.) 

Barium  sodium  selenoxyarsenate, 

BaNaAsO3Se+9H2O. 
Ppt.    (Weinland,  Z.  anorg.  1897,  14.  56.) 

Potassium  selenoxyarsenate,  2K2O,  2SeO3, 
As2O5+3H2O.  • 

Sol.  in  H2O  with  decomp.  (Weinland  and 
Barttlingck,  B.  1903,  36.  1403.) 

7K2O,10Seq3,2As2O5  +  llH2O.  Very  sol. 
in  H2O.  (Weinland  and  Barttlingck.) 

3K2O,  As2Se5-f  10H2O.    Easily  decomp.  by 


SILICIC  ACID 


801 


moisture.     Very  sol.   in  H2O.      (Clever,   Z 
anorg.  1895,  10.  126.) 

Rubidium  selenoxyarsenate,  2Rb2O,  2SeO3 

As2O5+3H2O. 

Sol.  in  H2O  with  decomp.  (Weinland  and 
Barttlingck.) 

Sodium  selenoxyarsenate,  Na3AsSeO3. 

Fairly  stable  in  air  and  in  aq.  solution. 
(Weinland,  B.  1896,  29.  1010.) 

Na3AsSeO3  +  12H2O.  Stable  in  the  air 
when  pure;  sol.  in  H2O  with  decomp.  (Wein- 
land, Z.  anorg.  1897,  14.  50.) 

Na3AsSeO3  +  12H2O.  Very  sol.  in  H2O; 
very  unstable.  (Szarvasy,  B.  1895,  28.  2657.) 

3Na2O,  3Na2Se,  As2O6+50H2O.  Easily 
sol.  in  H2O.  Solution  may  be  boiled  for  a 
long  time  without  decomp.  (Clever,  Z. 
anorg.  1895, 10. 136.) 

Selenoxyphosphoric  acid. 

Ammonium  /nselenmowoxyphosphate, 

(NH4)3PSe3O  +  10H2O. 
Ppt.    (Ephraim,  B.  1910,  43.  280.) 

Ammonium    hydrogen    /melenraonoxyphos- 

phate,  (NH4)5H(PSe3O)2+18H2O. 
Ppt.    (Ephraim.) 

Barium  hydrogen  efo'selen^'oxyphosphate, 

BaHPSe2O2  +  14H2O. 
Decomp.  in  moist  air.    (Ephraim.) 

Potassium   selenoxyphosphate,   K3PSe2.5Oi.6 

+H20. 

Decomp.  by  HNO3.  Insol.  in  alcohol  and 
ether.  (Ephraim.) 

Sodium  raowoselen^n'oxyphosphate, 

Na3PSeO3+20H2O. 
Decomp.  by  H2O.    (Ephraim.) 

Sodium  friselenwowoxyphosphate,  Na3PSe3O 

+  10H20. 

Sol,  in  H2O.  Decomp.  in  aq.  solution. 
Easily  sol.  in  cone.  NaOH+Aq.  (Muth- 
mann,  Z.  anorg.  1897,  13.  199.) 

Selenyl  bromide,  SeOBr2  (?). 
(Schneider,  Pogg.  129.  450.) 

Selenyl  bromide   sulphur  inoxide,    SeOBr2, 

SO3. 
(Prandtl,  Z.  anorg.  1909,  62.  242.) 

Selenyl  chloride,  SeO2Cl2. 

Easily  decomp.  by  H2O.  (Weber,  Pogg. 
118.  615.) 

Selenyl  sulphur  chloride. 
See  Sulphoselenyl  chloride. 


Selenyl  stannic  chloride,  2SeOCl,  SnCl4. 

Extremely  deliquescent.  Completely  sol. 
in  H2O.  (Weber,  B.  A.  B.  1866.  154.) 

Selenyl  titanium  chloride,  2SeOCl2,  TiCl4. 

Decomp.  by  H2O  with  separation  of  an 
insol.  residue.  Decomp.  by  NH4OH+Aq. 
(Weber,  B.  A.  B.  1865.  154.) 

Sesquiauramine. 
See  Sesquiaurainine. 

Sesquihydraurylamine,  (HOAu)3N,  NH8. 
See  £esgmhydraurylamine. 

Silicic  acid,  SiO2,  zH2O. 

See  also  Silicon  dioxide. 

Silicic  acid  is  sol.  in  1000  pts.  pure  H2O. 
(Kirwan.) 

When  pptd.  from  alkali  silicates +Aq  by 
CO2,  0.021  pt.  SiO2  remains  dissolved  in  100 
pts.  H2O.  (Struckmann,  A.  94.  341.) 

When  pptd.  as  above,  100  pts.  H2O  dissolve 
0.09  pt.  SiO2  in  3  days;  100  pts.  H2CO3+Aq 
dissolve  0.078  pt.  SiO2  in  3  days.  But  if 
heated  much  more  dissolves,  the  jelly  itself 
becoming  liquid,  such  jelly  containing  2.49 
pts.  SiO2  to  100  pts.  H2O.  This  solution  is 
not  pptd.  by  considerable  quantities  of  al- 
cohol, but  cone.  (NH4)2CO3,  NaCl,  or  CaCl2  + 
Aq,  etc.,  cause  gelatinization.  (Maschke,  J. 
pr.  68.  234.) 

Solubility  in  H2O  depends  on  the  amt.  of 
H2O,  in  presence  of  which  the  silicic  acid 
is  set  free  by  dil.  acids,  CO2,  or  alkali  salts+ 
Aq.  If  H2O  is  present  in  sufficient  quantity 
to  retain  the  silicic  acid,  much  more  will 
remain  in  solution  than  can  be  dissolved  by 
digesting  the  gelatinous  acid  with  H2O  after- 
wards. 1  pt.  SiO2  can  thus  be  held  in  solution 
by  500  pts.  H2O.  Presence  of  NH4OH, 
(NH4)2CO3,  or  NH4C1  (in  solutions  of  which 
SiO2  is  remarkably  insol.)  diminishes  the 
power  of  H2O  to  retain  SiO2  in  solution.  SiO2 
is  always  more  sol.  in  dil.  than  cone.  NH4OH 
+Aq.  (Liebig,  A.  94.  373.) 

Silicic  acid  from  the  coagulation  of  the  col- 
loidal form  (see  p.  802)  is  sol.  in  about  5000 
pts.  H2O  when  formed  from  a  1%  solution, 
and  10,000  pts.  when  formed  from  a  5%  solu- 
tion, but  is  insol.  after  being  dried.  (Graham, 
A.  121.  36.) 

Silicic  acid  is  more  sol.  in  dil.  acids  than  in 
H2O,  because,  when  acid  is  added  in  excess 
to  moderately  dil.  K2SiO3+Aq,  the  solution 
remains  clear,  but  if  only  enough  acid  is 
added  to  neutralize  the  base  present,  silicic 
acid  will  gradually  separate  out.  If  acid  is 
added  to  cone.  K2SiO3+Aq,  silicic  acid  sep- 
arates out  insol.  in  excess  of  acid,  but  if 
20-30  pts.  H2O  are  present  to  1  pt.  K2SiO3, 
and  an  excess  of  acid  added  at  once,  the  silicic 
acid  will  remain  in  solution.  This  result  is 
obtained  with  HC1,  HNO3,  H2SO4,  or 


802 


SILICIC  ACID 


HC2H3O2  + Aq .  These  solutions  may  dissolve 
a  neutral  salt  until  saturated  and  no  silicic 
acid  will  separate  out.  Therefore  it  is  the 
acid  that  holds  the  SiO2  in  solution,  and  not 
the  H2O.  (C.  J.  B.  Karsten,  (1826)  Pogg. 
6.  353.) 

Even  CO2  has  the  power  of  holding  SiO2 
in  solution.  (Karsten,  I.  c.) 

Solubility  in  acids  of  silicic  acid  of  Struck- 
mann  (see  above):  100  pts.  dil.  HCl+Aq  of 
1.088  sp.  gr.  dissolve  0.0172  g.  SiO2  in  11  days; 
100  pts.  H2O  sat.  with  CO2  dissolve  0.0136  g. 
SiO2  in  7  days. 

Silicic  acid  obtained  by  passing  SiF4  into 
H2O  is  sol.  while  still  moist  in  11,000  pts. 
cold,  and  5500  pts.  boiling  HCl+Aq  of  1.115 
sp.  gr.  (Fuchs,  A.  82.  119.) 

Silicic  acid  at  the  moment  of  separation  (as 
in  dissolving  cast-iron,  steel,  etc.)  is  abun- 
dantly sol.  in  aqua  regia  (3  pts.  HCl+Aq  of 
sp.  gr.  1.13  and  1  pt.  HNO3+Aq  of  sp.  gr. 
1.33).  (Wittstein,  Z.  anal.  7.  433.) 

The  aq.  solution  obtained  by  the  hydroly- 
sis of  ethyl  silicate  is  more  stable  in  acids + 
Aq  or  alkali  than  in  pure  H2O.  (Jordis,  Z. 
anorg.  1903,  35.  16.) 

NH4OH+Aq  dissolves  considerable  freshly 
precipitated  silicic  acid,  (NH4)2CO3  only  a 
very  little.  (Karsten,  Pogg.  6.  357.) 

Dry  or  ignited  SiO2  is  sol.  in  NH4OH  + 
Aq.  100  pts.  NH4OH+Aq  containing  10% 
NHs  dissolve:  0.714  pt.  SiO2  from  gelatinous 
silicic  acid;  0.303  pt.  from  artificially  dried 
silicic  acid;  0.377  pt.  from  amorphous  SiO2; 
0.017  pt.  from  quartz.  (Pribram,  Z.  anal.  6. 
119.) 

NH4OH+Aq  dissolves  0.382  pt.  SiO2  from 
dry  silicic  acid:  0.357  pt.  from  ignited  SiO2; 
0.00827  pt.  from  quartz.  (Souchay,  Z.  anal. 
11.  182.) 

Silicic  acid  precipitated  from  alkali  silicates 
+Aq  with  CO2  is  sol.  as  follows:  100  pts. 
pure  H2O  dissolve  0.021  pt.  SiO2;  100  pts 
(NH4)2CO3+Aq  containing  5%  (NH4)2CO3 
0.020  pt.;  100  pts.  containing  1%(NH4)2CO3; 
0.062  pt.;  100  pts.  NH4OH+Aq  containing 
19.2%  NH3,  0.071  pt.;  100  pts.  containing 
1.6%,  0.0986  pt.  (Struckmann,  A.  94. 
341.) 

100  pts.  NH4OH+Aq  (10%  NH3)  dissolve 
of:  crystallised  SiO2,  0.017  pt.;  amorphous 
SiO2,  ignited,  0.38  pt.;  amorphous  3SiO2, 
4H2O,  0.21  pt.;  amorphous  silicic  acid  in  form 
of  jelly,  0.71  pt.  Upon  evaporation  no  ppt 
is  formed,  even  when  80  mols.  SiO2  are  presenl 
to  1  mol.  NH3.  (Wittstein,  J.  B.  1866.  192.' 

Sol.  in  KOH  or  NaOH+Aq,  especially  i: 
warm.  (Dumas.) 

Sol.  in  K2SiO3  or  Na2SiO3+Aq.    (Fuchs.) 

Easily  sol.  in  boiling  Na2C03+Aq,  separat 
ing  as  a  jelly  on  cooling.  (Pfaff.) 

NH4C1  or  other  NH4  salts  ppt.  SiO2  from 
solution  in  Na2CO3+Aq. 

100  pts.  T12O  in  H2O  dissolve  4.17  pts 
: amorphous  SiO2  in  24  hours'  boiling.  (Flem 
lining,  Jena.  Zeit.  4.  36.) 


Sol.  in  butyl  amine.  (Wurtz,  A.  ch.  (3)  42. 
166.) 

Not  more  sol.  in  H2O  containing  sugar  than 
n  pure  H2O.  (Petzholdt,  J.  pr.  60.  368.) 

Soluble  silicic  acid. 

Colloidal  form  by  dialysis.    Solutions  con- 

;aining  4.9%  SiO2  may  be  evaporated  until 
they  contain  14 %  SiO2.  The  SiO2  is  separated 

rom  its  solution  thus  made  in  many  ways — 

(1)  By  standing.     This  happens  the  more 
easily  the  more  cone,  the  solution  is,  and  is 
mstened  by  heat.    A  10-12%  solution  gelatin- 
zes  at  ordinary  temp,  in  a  few  hours,  and 
mmediately  upon  heating.    A.  5-6%  solution 

may  be  kept  5-6  days,  a  2%  solution,  2-3 
months,  and  a  1%  solution  may  be  kept  2 
or  more  years  without  gelatinizing. 

(2)  When  the  solution  is  evaporated  to  dry- 
ness  in  vacuo  at  15°  a  transparent  glass  is  left 
which  is  insol.  in  H2O. 

(3)  The  coagulation  of  colloidal  silicic  acid 
is  accelerated  by  powdered  graphite  and  other 
indifferent  bodies,  and  it  is  brought  about  in  a 
few  minutes  by  a  solution  of  'the  alkali  car- 
bonates,   even   when   only  Vio,ooo  pt.    of   the 
carbonate  is  present.    (Graham,  A.  121.  36.) 

(4)  Coagulation  is  also  brought  about  by 
passing  CO2  through  the  solution.    (Liebig.) 

CO2  does  not  cause  coagulation.  (Maschke.) 

Coagulation  is  not  caused  by  H2SO4,  HC1, 
HNO3,  HC2H3O2,  H2C4H4O6,  or  NH4OH  + 
Aq,  or  by  neutral  or  acid  salts+Aq.  (Gra- 
ham.) 

NaCl  and  Na2SO4+Aq  coagulate  the  solu- 
tion. (Maschke.) 

Alcohol,  sugar,  glycerine,  or  caramel  do 
not  coagulate. 

Soluble  A12O6H6,  Fe2O6H6,  albumen,  and 
casein  precipitate  soluble  SiO2.  (Graham,  A. 
121.  36.) 

The  jelly  from  colloidal  SiO2  is  very  sol.  in 
slightly  alkaline  H2O.  1  pt.  NaOH  in  10,000 
pts.  H2O  dissolves  in  an  hour  at  100°  an  amt. 
of  the  jelly  corresponding  to  200  pts.  SiO2. 
(Graham.) 

Other  colloidal  forms. 

Various  solutions  of  silicic  acid  may  be 
obtained  as  follows: 

The  jelly  formed  when  SiF4  is  passed 
through  H2O  dissolves  in  a  large  amt.  of  H2O, 
and  SiO2  separates  out  on  evaporation.  This 
is  still  sol.  in  H2O,  but  is  made  insol.  by  evap- 
oration with  HC1  or  H2SO4.  (Berzelius.) 

When  SiF4  is  absorbed  by  crystallized 
H3BO3,  and  the  HF  and  H3BO3  removed  by 
a  large  excess  of  NH4OH+Aq,  a  silicic  acid  is 
obtained  which  is  very  sol.  in  H2O.  The 
solution  is  not  decomp.  by  boiling,  but  on 
evaporation  an  insol.  powder  remains.  (Ber- 
zelius, A.  ch.  14.  366.) 

When  K2SiO3+Aq  is  precipitated  by  CuCl2, 
the  precipitate  washed  and  dissolved  in  HC1+ 
Aq,  the  solution  treated  with  H2S  filtered  and 
boiled,  a  solution  of  silicic  acid  is  obtained 


SILICATE,  ALUMINUM  CALCIUM 


803 


which  gelatinizes  with  KOH  or  NH4OH+Aq. 
(Doveri,  A.  ch.  (3)  21.  40.) 

When  Na2SiO3-|-Aq  containing  at  most  3% 
SiO2  is  saturated  with  HCl+Aq  of  1.10  sp. 
gr.,  and  Na2SiO3  added  until  the  solution  is 
slightly  opalescent  and  carefully  warmed  to 
30°,  a  gelatinous  mass  is  obtained  which  will 
dissolve  in  H2O  by  12-16  hours'  boiling  if 
treated  before  being  exposed  to  the  air.  The 
solution  is  slightly  opalescent.  The  solution 
can  be  evaporated  by  heat  until  it  contains 
6%  SiO2.  In  a  vacuum  or  over  H2SO4,  solu- 
tions containing  10%  may  be  obtained.  The 
electric  current,  freezing,  alcohol,  or  H2SO4 
precipitate  or  coagulate  the  solution.  (Kuhn, 
J.  pr.  59.  1.) 

SiS2  with  H2O  gives  off  H2S,  and  forms  a 
solution  of  SiO2  which,  after  dilution,  can  be 
kept  for  months.  But  when  boiled  or  evapo- 
rated, or  when  a  sol.  silicate  is  added,  it 
becomes  gelatinous.  It  leaves  an  insol. 
residue  when  evaporated  to  dryness.  (Fremy, 
A.  ch.  (3)  38.  314.) 

Various  forms  of  silicic  acid  have  been  de- 
scribed as  definite  compounds  of  SiO2  with 
varying  amounts  of  H2O,  but  it  is  doubtful  if 
any  true  definite  compounds  exist,  as  the  per- 
centage of  H2O  varies  with  the  moisture  of  the 
air  to  which  it  is  exposed.  (See  Ebelmen,  A. 
ch.  (3)  16.  129;  Doveri,  A.  ch.  (3)  21.  40; 
Fuchs,  A.  82.  19;  Merz,  J.  pr.  99.  177;  van 
Bemmelen,  B.  11.  2232,  etc.) 

Silicates. 

The  silicates  are  insol.  in  H2O  with  the  ex- 
ception of  the  alkali  salts,  and  these  are  sol. 
only  when  the  ratio  of  the  base  to  the  acid  is 
above  a  certain  limit. 

Aluminum  silicate,  2A12O3,  SiO2  +  10H2O. 

Min.  Collyrite.  Sol.  in  acids,  with  forma- 
tion of  SiO2,  zH2O.  Becomes  transparent  in 
H2O  and  is  decomp. 

4A12O3,  3SiO2.    Min.  DiUnite. 

A12O3,  SiO2.  Min.  Andalusite,  Chiastolite, 
Sillimanniie,  Disthene  or  Cyanite.  Insol.  in 
acids. 

+5-7  H2O.  Min.  Allophane.  Completely 
sol.  in  dil.  acids;  decomp.  by  cone,  acids  with 
separation  of  SiO2,  o;H2O. 

2A12O3,  3SiO2+4H2O.  Min.  Pholeri'.e.  In- 
sol. in  HNO3+Aq. 

+6H2O.    Min.  Glagerite. 

A12O3,  2Si02+2H2O.  Min.  Kaolin,  Clay. 
Insol.  in  dil.  HC1  or  HNO3+Aq;  moderately 
dil.  H2SO4+Aq,  when  heated  to  evaporation, 
extracts  A12O3  and  some  SiO2,  ana  leaves  the 
rest  of  the  SiO2,  sol.  in  boiling  Na2CO3+Aq. 
All  the  A12O3  is  dissolved  by  heating  with  5-6 
pts.  H2SO<  +  lpt.H2O  until  H4SO4  evaporates, 
and  then  treating  with  H2O. 

Quickly  attacked  by  H2SiF6+Aq. 

Decomp.  by  boiling  KOH+Aq,  with  resi- 
due of  SiO2.  (Rammelsberg.) 

KOH+Aq  extracts  ^  of  the  SiO2  (Malar 


guti);  is  converted  thereby  into  double  sili- 
cates of  K  and  Al,  which  are  sol.  in  HCl+Aq. 
(Lemberg.) 

Solubility  in  KOH  and  HC1  increased  if 
first  heated  to  a  low  glow.  (Glinka,  C.  C. 
1899,  II.  1063.) 

Colloidal  day.      (Schlosing,  C.  R.  79.  473.) 

+4H2O.    Halloysite.    Decomp.  by  acids. 

4A12O3,  9SiO2  +  12H2O.  Min.  Porcelain 
clay  from  Passau. 

A12O3,  3SiO2+3H2O.  Min.  Razoumoff- 
sklne. 

A12O3,  4SiO2+7H2O.  Min.  Montmoril- 
lonite.  Not  decomp.  by  HCl+Aq,  but  by 
hot  H2SO4. 

+H2O.  Min.  Pyrophyllite.  Not  decomp. 
by  H2S04. 

+3H2O.    Min.  Anauxite. 

2A12O3,  9SiO2+6H2O.    Min.  Cimolite. 

"Aluminum  silicafe"  is  insol.  in  acetone. 
(Naumann,  B.  1904,  37.  4328);  ethyl  acetate. 
(Naumann,  B.  1910,  43.  314.) 

Aluminum  barium  silicate,  A12O3,  BaO,  2SiO2 
+H20  (?). 

Min.  Edingtonite.  Decomp.  by  HCl+Aq 
with  separation  of  SiO2,  zH2O. 

5A12O3,  4BaO,  10SiO2.  (Fremy  and  Feil, 
C.  R.  85.  1033.) 

2A12O3,  4BaO,  7Si02.  Min.  Barylite.  Very 
si.  decomp.  by  alkali  carbonates +Aq.  (Blom- 
strand.) 

Aluminum  barium  potassium  silicate, 
A12O3,  (Ba,  K2)O,  5SiO2+2H2O. 

Min.  Harmot'ome.  When  finely  powdered, 
difficultly  decomp.  by  HCl+Aq  with  separa- 
tion of  pulverulent  SiO2,  zH2O. 

A12O3,  (Ba,K2)O. 4SiO2.  Min.  Hagalophane. 
Scarcely  attacked  oy  acids. 

Aluminum  caesium  silicate,  H2Cs2Al2Si5O16  (?) 
Min.  Pollucite.     Very  si.  decomp.  by  HC1+ 
Aq. 

Aluminum  calcium  silicate,  A12O3,  CaO,  2SiO2. 

Min.  Anorthite.  Completely  decomp.  by 
HCl+Aq  with  separation  of  pulverulent  SiO2, 
zH2O. 

Min.  Barsowite.  Instantaneously  decomp. 
by  HCl+Aq,  with  separation  of  gelatinous 
SiO2,  xH2O. 

+4H2O.  Min.  Gismondite.  Gelatinizes 
with  HCl+Aq. 

A12O3,  CaO,  3SiO2+3H2O.  Min.  Scolezite. 
Easily  sol.  in  HCl+Aq,  without  formation  of 
gelatinous  SiO2.  Sol.  in  H2C2O4+Aq  with 
pptn.  of  CaC2O4. 

Decomp.  by,  and  sol.  to  a  certain  extent  in 
H2CO3+Aq,  and  decomp.  also  even  by  pure 
H2O.  (Rogers,  Am.  J.  Sci.  (2)  5.  408.) 

+5H2O.  Min.  Levyn.  Decomp.  by  acids 
without  gelatinizing. 

A12O3,  CaO,  4SiO2+3H2O.  Min.  Capor- 
cianite.  Leonhardite.  Efflorescent.  Easily 


804 


SILICATE,  ALUMINUM  CALCIUM  FERRIC 


sol.  in  acids,  with  pptn.  of  gelatinous  SiO2, 


A12O3,  CaO,  4SiO2+4H2O.  Min.  Laumon- 
tite.  Easily  gelatinizes  with  HC1  or  HNO3+ 
Aq,  but  is  not  affected  by  H2SO4  unless  hot. 

A12O3,  CaO,  6SiO2+5H2O.  Min.  Epistil- 
bite.  Gelatinizes  with  cone.  HCl+Aq.  (Gold- 
schmidt,  Z.  anal.  17.  267.) 

Scarcely  decomp.  by  boiling  cone.  HC1+ 
Aq.  (Jannasch  and  Tenne,  Miner.  Jahrb. 
1880,  1.  43.) 

+6H2O.  Stilbite.  Heulandite.  Slowly 
but  completely  gelatinized  by  HCl+Aq. 

A12O3,  2CaO,  3SiO2+H2O.  Min.  Prehnite. 
Imperfectly  decomp.  by  acids  before  ignition, 
but  easily  afterwards. 

A12O3,  3CaO,  3SiO2.  Lime  alumina  garnet. 
Grossularite.  Partially  decomp.  by  acids 
before  ignition,  but  easily  afterwards. 

2A12O3,  CaO,  2SiO2+H2O.  Margarite. 
Not  attacked  by  acids. 

3A12O3,  4CaO,  6SiO2+H2O.  Zoisite.  Par- 
tially decomp.  by  HCl+Aq. 

4A12O3,  6CaO,  9SiO2.  Min.  Meionite. 
Completely  sol.  in  HCl+Aq. 

Aluminum    calcium    ferric    silicate,    2A12O3, 

4CaO,  Fe2O3,  6SiO2+H2O. 
Min.  Epidote.     Only  si.  attacked  by  HC1+ 
Aq  before  ignition. 

Aluminum  calcium  ferric  magnesium  silicate, 
Hu(Ca,  Mg)40(Al2,  Fe2)10Si35O147. 
Min.  Vesuvianite,  Idiocrase.    Only  partially 

decomp.  by  HCl+Aq  before  ignition. 

Aluminum  calcium  iron,  etc.,  silicate  borate, 

H2RI61(A12,  B2)3Si8O32. 
Min.  Axinite.    Not  attacked  by  HCl+Aq 
before  ignition. 

Aluminum  calcium  magnesium  silicate, 
4H4Ca2Mg8Si6O24,  5H2CaMgAl6O12  = 
15A12O3,   13CaO,  37MgO,  24SiO2  + 
13H20. 

Min.  Clintonite.  Completely  decomp.  by 
HCl+Aq  without  gelatinization. 

3H4Ca2Mg8Si6024,  4H2CaMgAl6O]2.  Min. 
Brandisite.  Not  attacked  by  HCl+Aq. 
Slowly  decomp.  by  boiling  cone.  H2SO4. 

5H4Ca2Mg8Si6O24,  8H2CaMgAl6O12.  Min. 
Xanthophyllite.  Very  si.  decomp.  by  hot 
HCl+Aq. 

3(Ca,  Mg)O,  A12O3,  2SiO2.  Min.  Gehlenite. 
Easily  decomp.  by  acids. 

Aluminum  calcium  potassium  silicate, 

(H,  K)2CaAl2Si5O15+6H2O. 

Min.  Chabosite.    Decomp.  by  HCl+Aq. 

(K2,  Ca)Al2Si3O10+4H2O.  Min.  Zeagonite. 
Completely  sol:  in  HCl+Aq. 

Aluminum  calcium  sodium  silicate,  3A12O3, 

8CaO,  Na2O,  9SiO2. 
Min.  -Sarcolite  Decomp.  by  acids. 


2A12O3,  12(Ca,Na2)O,  9SiO2  (?).  Min. 
Mellilite.  Gelatinized  by  acids. 

Na2CaAl4Si2Oi2  (?).    Min.  Margarite. 

Na2CaAl4Sii0O28.  Min.  Faiijasite.  De- 
comp. by  HCl+Aq. 

(Na2,  'Ca)Al2Si4O12.  Min.  Gmelinite.  De- 
comp. by  HCl+Aq. 

(Ca,  Na2)Al2Si6Oi9+6H2O.  Min.  Foresite. 
Difficultly  decomp.  by  HCl+Aq. 

(Ca,  Na2)Al2Si2O8+2>£H2O.  Min.  Thom- 
sonite.  Gelatinizes  with  HCl+Aq. 

zNa2Al2Si6O16,  ?/CaAl2Si2O8.  Min.  Oligo- 
clase,  Labradorite.  SI.  decomp.  by  acids, 
more  easily  the  larger  the  amt.  of  Ca  present. 

Aluminum  calcium  sodium  silicate  sulphate, 

2(Na2,  Ca)Al2(SiO4)2,  (Na2,  Ca)SO4. 
Min.  Hauyn.    Gelatinizes  with  HCl+Aq. 

Aluminum  glucinum  silicate,  A12O3,  3G1O, 
6Si02. 

Min.  Beryl.  Emerald.  Not  decomp.  by 
acids,  excepting  partially  by  H2SO4  after  be- 
ing ignited. 

A12O3,  2G1O,  2SiO2+H2O.  Min.  Euclase. 
Not  attacked  by  acids. 

Aluminum  ferrous  silicate,  Al2Fe(SO4)3. 

Min.  Garnet.    SI.  decomp.  by  HCl+Aq. 

H2FeAl2SiO7.  Min.  Chloritoid.  Not  at- 
tacked by  HCl+Aq.  Completely  decomp. 
by  H2S04. 

A12O3,  3FeO,  3SiO2+3H2O.    Min.  Voiglite. 


Aluminum  iron  lithium   potassium   silicate, 

K3Li3Fe4Al12Si20O65. 
Min.  Zinnwaldite.    SI.  decomp.  by  acids. 

Aluminum  ferrous  magnesium  silicate, 

%6A12O3,  3(Mg,  Fe)O,  6SiO2+H2O. 
Min.  Siaurolite.    Not  attacked  by  acids. 

Aluminum  ferric  magnesium  silicate, 

2(A12,  Fe2)O3,  2MgO,  5SiO2. 
Min.  Cordierite.     SI.  attacked  by  acids. 
+rcH2O.    Min.  Esmarkite,  Chlorophyllite. 

Aluminum  ferrous  manganous  silicate,  A12O3, 

FeO,  2MnO,  3SiO2. 
Min.  Partschinite. 

Aluminum  ferrous  sodium,  etc.,  silicate  borate, 

)  (B2).Si4O20  +  R1?(Al2)2(B2)Si4O2o, 


etc. 

Min.  Tourmaline.  Not  decomp.  by  HC1+ 
Aq;  very  si.  decomp.  by  H2SO4. 

Aluminum  lithium  silicate,  A12O3,  Li2O,  5Si02. 

Not  attacked  by  acids.  (Hautefeuille, 
C.  R.  90.  541.) 

A12O3,  Li2O,  6SiO2. 

A12O3,  Li2O,  4SiO2.  [Min.  Spodumene.  Not 
attacked  by  acids. 


SILICATE,  OESIUM 


805 


4A12O3,  3Li2O,  30SiO2.  Min.  Petalite.  .Not 
attacked  by  acids. 

Aluminum  lithium  potassium  silicate, 

(Li,  K)10Al10Sii6O52. 
Min.  Lepidolite.    SI.  decomp.  by  acids. 

Aluminum  magnesium  silicate,  5A12O3, 4MgO, 

2SiO2. 
Min.  Sapphirine. 

Aluminum  magnesium  potassium  silicate, 
zH4K2Al6Si6O24,  2/Mg12Si6O21. 

Min.  Lepidomelane.  Easily  decomp.  by 
HC1  or  HNO3+Aq,  with  residue  of  a  skeleton 
of  SiO2. 

3A12O3,  12MgO,  2K2O,  12SiO2+H2O.  Min. 
Anomite. 

7A12O3,  35MgO,  7K2O,  36SiO2.  Min. 
Phlogopite. 

Aluminum  manganous  silicate,  2A12O3,  6MnO, 

6SiO2. 

Not  decomp.  by  very  dil.  HCl+Aq.  (Gor- 
geu,  C.  R.  97.  1303.) 

Aluminum  potassium  silicate,  A12O3,  K2O, 
SiO2. 

Very  slowly  decomp.  by  cold  H2O;  12%  is 
dissolved  by  hot  H2O.  Sol.  in  alkali  hydrox- 
ides+Aq,  but  insol.  in  carbonates +Aq. 

K2O,  A12O3,  2SiO2.  Insol.  in  cold  H2O,  but 
6%  dissolves  on  boiling.  Sol.  in  dil.  acids. 
Insol.  in  alkali  hydroxides  or  carbonates  +Aq. 
(Gorgeu,  A.  ch.  (6)  10.  45.) 

K2O,  A12O3,  3SiO2+3H2O.  Easily  sol.  in 
HNO3+Aq.  (Deville,  A.  ch.  (3)  61.  313.) 

K2O,  A12O3,  4SiO2.  Min.  Leucite.  De- 
comp. by  HCl+Aq  with  separation  of  pul- 
verulent SiO2. 

+4H2O.    Ppt.    (Deville,  C.  R.  64.  324.) 

H4K2Al6Si6O24.  Min.  Muscovite,  "Mica." 
Not  attacked  by  HC1  or  H2SO4+Aq. 

K2Al4Si5O17+3H2O.  Min.  Finite.  Partly 
decomp.  by  HCl+Aq. 

K2Al2Si6Oi6.  Min.  Orthoclase.  Feldspar. 
Scarcely  attacked  by  acids.  Slowly  sol.  in 
H2SO4  or  HCl+Aq  when  finely  powdered. 
(Rogers.) 

Aluminum  potassium  sodium  silicate, 

K2Al2(SiO3)4,  5Na2Al2(SiO4)2  (?). 
Min.  Nepheline.    Decomp.  by  HCl+Aq. 

Aluminum  silver  silicate,  Al2Ag4Si2O9. 

Insol.  in  NH4OH+Aq.    (Silber,  B.  14.  941.) 
Al6Ag2Na4Si6O4.    As  above.    (Silber.) 

Aluminum  sodium  silicate,  A12O3,  Na2O,  SiO2. 

Insol.  in  cold  H2O,  but  38-40%  dissolves  in 
hot  H2O.  (Gorgeu.) 

A12O3,  Na2O,  2SiO2.  Insol.  in  cold  H2O; 
boiling  H2O  dissolves  1-2%.  Sol.  in  HC1  or 
HNO3  diluted  with  10-20  vols.  H2O.  Insol. 


in  alkali  hydroxides  or  carbonates +Aq. 
(Gorgeu,  A.  ch.  (6)  10.  145.) 

Not  attacked  by  H2O.    (Silber,  B.  14.  941.) 

+3H2O.  Easily  sol.  in  HCl+Aq.  (v. 
Ammon.) 

A12O8,  Na2O,  3SiO2+3H2O.  Decomp.  by 
acids.  (Deville,  A.  ch.  (3)  61.  326.) 

A12O3,  Na2O,  4SiO2+3H2O.  Easily  sol.  in 
HCl+Aq.  (v.  Ammon.) 

2A12O3,  3Na2O,  3SiO2.  Insol.  in  cold  H2O, 
but  27-30%  dissolves  on  boiling.  (Gorgeu.) 

H4Na2Al6Si6O24.  Min.  Bafagonite.  De- 
comp. by  cone.  H2SO4. 

Na2Al2Si4O12+2H2O.  Min.  Anaclite. 
Readily  decomp.  by  HCl+Aq. 

Na2Al2Si3Oio+2H2O.  Min.  Natrolite.  Sol. 
in  H2O  with  separation  of  SiO2.  Also  sol.  in 
H2C2O4+Aq. 

Na?Al2Si«Oi6.  Min.  Albite.  Not  attacked 
by  acids. 

Aluminum  sodium  silicate  chloride, 

3Na2Al2(SiO4)2,  2NaCl. 
Min.  Sodalite.     Easily   decomp.  by  HC1, 
and  HNOs+Aq. 

Aluminum  sodium  silicate  sulphate, 

3Na2Al1(SiO4)2,  Na2SO4. 
Min.  Nosean.     Easily  decomp.  by  HC1  + 
Aq. 

Aluminum  sodium  silicate  sulphide. 
See  Ultramarine. 

Barium  silicate,  BaSiO3. 

Somewhat  sol.  in  boiling  H2O.  Completely 
sol.  in  dil.  HCl+Aq.  (v.  Ammon.) 

+6H2O,  or  7H2O.  Boiling  H2O  decom- 
poses, and  dissolves  about  }/%  the  weight  of 
this  substance,  (le  Chatelier,  C.  R.  92.  931.) 

2BaO,  SiO2.  Decomp.  by  H2O  into  BaSiO3 
+6H2O.  (Laudrin.) 

Bismuth  silicate,  2Bi2O3,  3SiO2. 

Min.  Eulytite.    Decomp.  by  HCl+Aq. 

Bismuth  ferric  silicate,  Bi2Fe4Si4Oi7. 
Min.  Bismuthoferrite. 

Boron  calcium  silicate. 

See  Borate  silicate,  calcium,  and  Silicate 
borate,  calcium. 

Cadmium  silicate,  CdSi03+l^H2O. 

Sol.  in  HCl+Aq  with  deposition  of  pul- 
verulent SiO2,  zH2O.  (Rousseau  and  Tite, 
C.  R.  114.  1262.) 

Caesium  silicate,  Cs2SiO3. 

(Kahlenberg,  J.  phys.  Chem.  1898,  2. 
82.) 


806 


SILICATE,  CALCIUM 


Calcium  silicate,  CaSiO3. 

Slowly  sol.  in  H2O;  sol.  in  HCl+Aq. 

Sol.  in  about  100,000  pts.  H2O.     (Gorgeu. 

A.  ch.  1885,  (6)  4.  550.) 

100  cc.  sat.  aq.  solution  of  air  dried  cal- 
cium silicate  contains  0.0046  g.  CaO  =  0.0095 
g.  CaSiO3  at  17°.  (Weisberg,  Bull.  Soc. 
1896,  (3)  15.  1097.) 

100  cc.  sat.  solution  of  air  dried  calcium 
silicate  in  10%  sugar  solution  at  17°  contains 
0.0065  g.  CaO  =  0.0135  g.  CaSiO3;  20%  sugar 
solution,  0.0076  g.  CaO  =  0.0175  g.  CaSiO,. 

After  boiling  and  filtering  hot,  10%  sugar 
solution  contains  0.0094  g.  CaO  =  0.0195  g. 
CaSiO3;  20%  sugar  solution,  0.0120  g.  CaO  = 
0.0249  g.  CaSiO3.  (Weisberg.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate:  (Naumann, 

B.  1910,  43.  314.) 

4CaO,  3SiO2.    (Laudrin.) 

5CaO,  3SiO2+5H2O.  When  freshly  pre- 
cipitated is  somewhat  sol.  in  H2O  and  easily 
decomp.  by  HCl+Aq.  (v.  Ammon.) 

CaO,  3SiO2+2H2O.  (Hjeldt,  J.  pr.  94. 
129.) 

2CaO,  9SiO2+3H2O.    Ppt. 

CaSiO3.  Min.  Wollastonite.  Gelatinizes 
with  HCl+Aq. 

CaSi2O5+2H2O.  Min.  Okenite.  Easily  de- 
comp. by  cold  HCl+Aq  when  powdered. 

Calcium  glucinum  silicate  sodium  fluoride, 

(Ca,  Gl)i5Sii4O43,  6NaF. 
Min.    Leucophane. 
7(Ca,  Gl)3Si2O7,  6NaF.    Min.  Melinophane. 

Calcium  ferrous  silicate,  CaSiO3,  FeSiO3. 

Min.  Hederibergite,  Pyroxene.  SI.  decomp. 
by  acids. 

Calcium  ferric  silicate,  Ca3Fe2(SiO4)s. 

Min.  Garnet.    SI.  decomp.  by  HCl+Aq. 

2CaSiO3,  11  Fe2(SiO3)3.  Min.  Szaboite. 
SI.  attacked  by  HCl+Aq,  and  still  less  by 
H2SO4+Aq. 

Calcium    ferroferric    silicate,    2CaO,    4FeO, 
Fe2O3,  4SiO2+H2O  =  H2Ca2Fe4Fe2Si4O18. 
Min.    Lievrite,  Ilvaite.     Easily   gelatinizes 
with  HCl+Aq. 

Calcium  ferrous  magnesium  silicate, 

(Ca,  Fe,  Mg)SiO3. 

Min.  Amphibole,  Hornblende,  Asbestos, 
Actinolite,  Tremolite.  Only  si.  attacked  by 
acids. 

Calcium  ferroferric  sodium  silicate,  CaSiO3, 

FeSiO3,  Fe2(SiO3)3,  Na2SiO3. 
Min.  Aegirite. 

Calcium  magnesium  silicate,  CaO,  MgO, 
4SiO2. 

(Mutschler,  A.  176.  86.) 

Ca2SiO4,  Mg2SiO4.  Min.  Monticellite. 
Completely  sol.  in  dil.  HCl+Aq. 


(Oa,Mg)SiO3.  Min.  Diopside,  Pyroxene. 
Very  si.  attacked  by 'acids. 

Calcium    manganous    silicate,    CaSiO3, 

2MnSiO3. 
Min.  Bustamite. 

Calcium  potassium  silicate. 
See  under  Glass. 

Calcium  sodium  silicate,  (Ca,  Na2,  H2)SiO8. 
Min.  Pectolite.  Decomp.  by  HCl+Aq. 
See  under  glass. 

Calcium  sodium  silicate  zirconate, 

Na4Ca(Si,Zr)9O2i +9H2O. 
Min.  Wohlente.    Decomp.  by  HCl+Aq. 

Calcium  uranyl  silicate,  3CaO,  5UO3,  6SiO2  + 

18H2O. 

Min.  Uranophane.     Gelatinizes  with  acids. 
CaO,  3UO3,  3SiO2+9H2O.    Min.  Uranotile. 

Calcium  silicate  chloride,  2CaO,  SiO2,  CaCl2. 
Insol.  in  H2O  or  alcohol.    Sol.  in  HCl+Aq. 
(le  Chatelier,  C.  R.  97.  1510.) 

Calcium  silicate  fluoride,  2CaO,  3SiO2,  6CaF2. 
(Deville,  C.  R.  62.  110.) 

Calcium  silicate  potassium  fluoride, 

4H2CaSi2O6,  KF+4H2O. 
Min.    Apophyllite..    Decomp.  by  HCl+Aq. 

Calcium  silicate  stannate. 
See  Silicostannate,  calcium. 

Calcium  silicate  titanate,  CaO,  SiO2,  TiO2. 
(Hautefeuille,  A.  ch.  (4)  4.  154.) 
Min.  Titanite.     Incompletely  decomp.  by 

HCl+Aq,  wholly  by  H2SO4+Aq. 

Cerous  silicate,  Ce2(SiO3)3. 

More  or  less  attacked  by  HC1,  HNO3,  or 
H2SO4+Aq,  according  to  the  concentration. 
(Didier,  C.  R.  101.  882.) 

Cerium  didymium  lanthanum  silicate, 

2(Ce,La,Di)2O3,  3SiO2. 
Min.  Cerite.    Gelatinizes  with  HCl+Aq. 

Cerium  glucinum  yttrium  silicate, 

(Y,Ce,Gl)2SiO5. 

Min.  Gadolinite.  Easily  gelatinized  by 
HCl+Aq. 

Cerous  silicate  chloride,  2Ce2O3,  3SiO2, 

4CeCl3  =  Ce4(SiO4)3,  4CeCl3. 
Insol.  in  H2O,  but  slowly  decomp.  thereby. 
(Didier,  C.  R.  101.  882.) 


SILICATE,  MAGNESIUM,  FLUOSILICATE 


807 


Cobaltous  silicate,  Co2SiO4. 

Gelatinizes  with  HCl+Aq.  (Bourgeois,  C. 
R.  108.  1077.) 

Cupric  silicate,  CuH2SiO4. 

Min.  Dioptase.  Sol.  in  HC1,  HNO3,  or 
NH4OH+Aq  with  separation  of  SiO2.  Not 
attacked  by  KOH+Aq. 

CuSiO3+2H2O.  Min.  Chrysocolla.  De- 
comp. by  HCl+Aq. 

+3H2O.  Min.  Asperolite.  Easily  de- 
comp. by  HCl+Aq. 

"Cupric  silicate"  is  insol.  in  methyl  acetate. 
(Naumann,  B.  1909,  42.  3790.) 

Cupric  silicate  ammonia,  CuSi2O5,  2NH3. 
Ppt.     (Schiff,  A.  123.  38.) 

Glucinum  silicate,  Gl2Si04. 

Min.     Phenacite.     Not  attacked  by  acids. 

Glucinum  ferrous  manganous  silicate  ferrous 
manganous  sulphide,  3(G1,  Fe,  Mn)2SiO4, 
(Mn,  Fe)S. 
Min.    Helvine.    Decomp.  by  HCl+Aq. 

Iron  (ferrous)  silicate,  Fe2SiO4. 

Min.     Fayalite.     Gelatinizes  with  HC1+ 

FeSiO3.     Min.     Grunerite. 

+6H2O.    Min.    Chlorophite. 

4FeO,  SiO2.     (Zobel,  Dingl.  154.  111.) 

Iron  (ferric)  silicate,  Fe2Si3O9+5H2O. 

Min.  Nontronite.  Gelatinizes  with  hot 
acids. 

4Fe2O3,  9SiO2  +  18H2O.    Min.    Hisingerite. 

2Fe2O3,  9SiO2+2H2O.  Min.  Anthosider- 
ite. 

Iron  (ferroferric)  magnesium  silicate, 

(Fe,  Mg)3Fe2Si2010+4H20. 
Min.        Cronstadtite.       Gelatinizes      with 
acids. 

Iron  (ferroferric)  sodium  silicate,  5Na2SiO3, 

2FeSiO3,  4Fe2(SiO3)3. 
Min.    Aknite.     SI.  decomp.  by  acids. 

Iron  (ferrous)  magnesium  silicate,  Fe2SiO4, 
Mg2SiO4. 

Min.  Olivene,  Chrysolite,  Peridote.  Gelat- 
inizes with  HC1  or  H2SO4+Aq. 

(Fe,  Mg)SiO3+3/2H2O.   Min.   Picrophyllite. 

+  i^H2O.     Min.     Monradite. 

(Fe,Mg)SiO3.  Min.  Bronzite,  Hypersthene. 
Not  attacked  by  acids. 

zMgSiOs,  2/FeSiO3.  Min.  Anthophyllite. 
Not  attacked  by  acids. 

Iron  (ferrous)  manganous  silicate,  Fe2SiO4, 

Mn2SiO4. 

Min.  Knebelite.  Gelatinizes  with  HC1+ 
Aq. 


Iron  (ferrous)  manganous  silicate  chloride, 

7(Fe,Mn)SiO3,  (Fe,Mn)Cl2+5H2O. 
Min.     Pyrosmalite.      Completely  decomp. 
by  cone.  HNO3+Aq. 

Iron   (ferric)   potassium   silicate,   Fe(SiOs)3, 

K2SiO3. 
(Hautefeuille  and  Perrey,  C.  R.  107.  1150.) 

Iron  (ferric)   sodium  silicate,  Na2Fe2Si4Ou. 
Min.      Crokydolite.      Not     attacked     by 
acids. 

Lead  silicate. 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329);  methyl  acetate.  (Naumann,  B.  1909, 
42.  3790.) 

See  under  Glass. 

Lithium  'silicate,  Li2Si5On. 

Li4SiO4. 

Li2SiO3.  More  stable  towards  H2O  than 
the  other  alkali  metasilicates.  (Rieke  and 
Endell,  C.  C.  1911,  I.  7.) 

Decomp.  by  boiling  H2O  and  acids.  (Frie- 
del,  C.  C.  1901,  II.  89.) 

Scarcely  attacked  by  cold  H2O.  (Friedel, 
Bull.  Soc.  Min.  1901,  24.  141.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1904,  37.  3601);  methyl  acetate.  (Naumann, 
B.  1909,  42.  3790.) 

Magnesium  silicate,  Mg3Si2O7+2H2O. 

Min.  Serpentine.  Decomp.  by  HCl+Aq, 
more  easily  by  H2SO4. 

Min.    Chrysotile. 

Mg4Si3Oio+6H2O.  Min.  Gymnite,  Soap- 
stone.  Decomp.  by  H2SO4. 

MgSiO3.  Not  completely  decomp.  by 
HCl+Aq. 

+  J^H2O.  Min.  Aphrodite.  Decomp.  by 
hot  acids. 

+  3/£H2O.    Min.    Picrosmine. 

-flVsHaO.    Sol.  in  dil.  acids,    (v.  Ammon.) 

Min.     Forsterite. 

3MgO,  4SiO2+H2O  or  4MgO,  5SiO2  + 
^H2O.  Min.  Talc  or  Steatite.  Not  at- 
tacked by  HC1  or  H2SO4+Aq. 

Mg5Si6O17+4H2O.  Min.  Spadaite.  De- 
comp. by  cone.  HCl+Aq. 

Mg2Si3O8+4H2O.  Min.  Meerschaum. 
Decomp.  by  HCl+Aq. 

"Magnesium  silicate,"  is  insol.  in  methyl 
acetate.  (Naumann,  B.  1909,  42.  3790.) 

Magnesium  potassium  silicate, 

MgO,  K2O,  3SiO2. 

Easily  sol.  in  acids  with  decomp.  (Du- 
boin,  C.  R.  1895,  120.  681.) 

Magnesium    silicate    fluosilicate,    Mg5Si2O9, 

Mg5Si2F18. 

Min.  Humite,  Chondrodite.  Gelatinizes 
with  HC1  or  H2SO4+Aq. 


SILICATE,  MANGANOUS 


Manganous  silicate,  Mn2SiO4. 

Min.  Tephroite.  Decomp.  by  HCl+Aq 
with  formation  of  a  stiff  jelly. 

MnSiO3.  Min.  Rhodonite,  Hermannite. 
Not  attacked  by  HCl+Aq. 

Mn4Si3Oio+2H2O.       Min.       Friedelite. 
Easily  gelatinized  by  HCl+Aq. 

"Manganous  silicate"  is  insol.  in  ethyl 
acetate.  (Naumann,  B.  1910,  43.  314.) 

Manganous  zinc  silicate,   (Mn,Zn)2SiO4. 
Min.    Troostite. 

Manganous  silicate  chloride,  MnSiO3,  MnO. 

MnCl2. 
Decomp.  by  H2O.    (Gorgeu.) 

Nickel  silicate,  Ni2Si04. 

Easily  decomp.  by  acids.  (Bourgeois,  C.  R. 
108.  1077.) 

Potassium  silicate,  K2SiO3. 

Completely  sol.  in  H2O.  (Ordway,  Sill. 
Am.  J.  (2)  33.  34.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

K2Si2O5.  Sol.inH2O.  Conc.K2Si24O5+Aq 
contains  28%  of  the  salt,  and  has  sp.  gr.  1.25. 
(Fuchs.) 

Hydroscopic.  Decomp.  at  once  by  H2O. 
(Morey,  J.  Am.  Chem.  Soc.  1914,  36.  222.) 

K2Si8O17.    Partially  sol.  in  H2O  as  K2SiO3. 

K2Si24O49  +  16H2O.  Insol.  in  H2O.  (Forch- 
hammer.) 

The  K  silicates  are  pptd.  from  their  aqueous 
solution  by  alcohol  with  partial  decomp.,  but 
less  readily  than  Na  silicates. 

More  sol.  in  H2O  than  the  corresponding 
Na  salts.  (Ordway,  Sill.  Am.  J.  (2)  32.  155.) 

Solution  can  be  obtained  which  is  perfectly 
clear  when  4^SiO2  are  present  to  1K2O,  if 
there  are  no  impurities  present.  (Ordway.) 

The  K  silicates  resemble  the  Na  salts, 
which  see  for  further  data. 

Potassium  hydrogen  silicate,  KHSi2O6. 

Not  readily  affected  by  H2O,  even  by  treat- 
ment at  100°  for  several  hours. 

Decomp.  by  heating  with  dil.  HC1.  (Morey, 
J.  Am.  Chem.  Soc.  1914,  36.  222.) 

Potassium  zinc  silicate. 

Sol.  in  KOH+Aq.     (Schindler.) 

K2O,  6ZnO,  4Si02.   Sol.  in  HCl+Aq.    (Du- 

boin,  C.  R.  1905,  141.  255.) 
8K2O,  9ZnO,  17SiO2.     Sol.  in  HCl+Aq. 

(Duboin.) 

Potassium    zirconium    silicate,    K2O,    ZrO2, 

2Si02. 
Decomp.  by  HCl+Aq.    (Melliss.) 

Rubidium  silicate,  Rb2SiO3. 

(Kahlenberg,  J.  phys.  Chem.  1898,  2.  82.) 


Silver  silicate,  Ag2SiO3. 

Decomp.  by  all  acids;  sol.  in  NH4OH+Aq. 
(Hawkins,  Sill.  Am.  J.  139.  311.) 

Sodium  silicate,  Na2SiO3. 

Rapidly  decomp.  by  H2O.  (Morey,  J. 
Am.  Chem.  Soc.  1914,  36.  224.) 

Insol.   in   methyl   acetate.      (Naumann, 
B.  1909,  42.  3790.) 

+5,   6,   and  8H2O.    Easily  sol.   in  H2O. 

+9H2O.  Solubility  in  3^-N  NaOH  + 
Aq. 

100  ccm.  of  the  solution  contain  25.56  g. 
Na2Si03+9H2Oat  17.5.° 

Sp.  gr.  of  the  solution  =  1.1 29.  (Vester- 
berg,  C.  C.  1913.  777.) 

100  ccm.  of  a  sat.  solution  of  sodium  sili- 
cate in  Y2-N.  NaCl+Aq.  contain  3.83  g. 
Na2SiO3+9H2O  at  17.5.°  Sp.  gr.  of  solution 
=  1.15. 

100  ccm.  of  a  sat.  solution  of  sodium  silicate 
in  sat.  NaCl+Aq  contain  20.64  g.  Na2SiO3 
+9H2O  at  17.5°.  (Vesterberg.) 

Na2Si2O6.    Sol.  in  H2O. 

Slowly  decomp.  by  cold  H2O.  (Morey 
J.  Am.  Chem.  Soc.  1914,  36.  223.) 

Na4Si6012. 

Na2Si3O7. 

Na2Si4O9.    Slowly  sol.  in  H2O. 

+  12H2O. 

Above  compounds  are  all  more  or  less 
indefinite. 

Water  glass.  zNa2O,  ?/SiO2+zH2O.  Sol. 
in  H2O,  but  solution  is  decomposed  by  all 
weak  acids,  even  CO2. 

Fused  water  glass  is  but  little  acted  on  by 
cold  H2O,  but  when  pure,  easily  dissolves  in 
H2O  by  long  boiling.  (Ordway,  Am.  J.  Sci. 
(2)  32.  337.) 

When  the  SiO2  is  present  in  greater  propor- 
tion than  in  Na2O,  3SiO2,  it  is  very  difficult 
to  dissolve  in  H2O. 

Na  silicate  is  less  easily  sol.  in  H2O  than 
the  corresponding  K  compound. 

Solubility  of  water  glass  in  H2O  is  much 
impaired  by  earthy  impurities,  so  that  traces 
have  great  effect  in  preventing  the  solubility. 

NH4  salts  decomp.  water  glass  solutions. 
A  solution  containing  l/$%  Na2SiO3  is  scarcely  . 
precipitated    by     NH4C1,     but     easily     by 
NH4NO3.    (Fluckinger.) 

Precipitated  by  NH4OH+Aq  as  Na2SiO3. 

Many  sodium  and  potassium  salts,  espe- 
cially the  chlorides  and  acetates,  form  precipi- 
tates in  solutions  of  water  glass;  these  pre- 
cipitates are  larger  the  more  concentrated 
the  solution  is,  and  the  greater  amount  of 
SiO2  it  contains.  Heating  hastens  the  pre- 
cipitation by  chlorides,  nitrates,  and  sul- 
phates, but  delays  that  by  acetates.  KOH  + 
Aq  does  not  precipitate. 

Cold  sat.  Na2SO4+Aq  does  not  precipitate 
even  on  heating,  but  1  pt.  anyhydrous  Na2SO4 
dissolved  in  2  pts.  H2O  precipitates  a  hot 
solution  of  Na2SiO3. 


SILICATE,  ZINC 


809 


NaNO?  dissolved  in  1  pt.  H2O  precipitate 
Na2SiO3+Aq  of  1.392  sp.  gr.;  NaNO3  in  2 
pts.  H2O  when  mixed  with  a  solution  of 
Na2SiO3,  as  above,  if  the  two  are  present  in 
equal  vols.,  causes  no  ppt.  in  the  cold,  but 
solidifies  when  warmed  to  54°,  and  redis- 
solves  on  cooling  rapidly,  but  if  2  vols.  NaNO3 
+Aq  are  present  to  1  vol.  Na2SiO3+Aq, 
the  precipitate  dees  not  disappear  on  cooling. 

If  1  pt.  NH4OH+Aq  (0.921  sp.  gr.)  is 
added  to  10  pts.  Na2SiO3+Aq,  no  ppt.  forms, 
but  by  increasing  the  amt.  of  NH4OH+Aq 
to  2  pts.,  the  greater  pt.  of  the  Na2SiO3  is 
pptd.,  but  redissolves  on  heating  to  90°,  separ- 
ating again  on  cooling.  When  1  pt.  NH4OH 
+Aq  is  added  to  6-8  pts.  Na2SiO3+Aq 
and  heated  to  30°,  a  clear  liquid  is  formed 
which  separates  into  two  layers  at  ordinary 
temp. 

The  most  sol.  K,  Na,  Li,  and  NH4  salts 
separate  SiO2  from  cone.  Na2SiO2+Aq. 
Most  of  these  salts  lose  this  power  by  dilu- 
tion, but  the  NH4  salts  and  KSON  keep  this 
power  until  the  solution  is  very  dil.  This  is 
especially  the  case  with  NH4C1  and  NH4NO3. 

Bromine,  chlorine,  propyl  amine,  crecsote, 
phenole  dissolved  in  glycerine,  chloral  hy- 
drate, dil.  albumen  solution,  and  glue  solu- 
tion ppt.  SiO2  from  Na2SiO3+Aq;  but  sugar, 
dextrine,  glycerine,  urea,  si.  alkaline  solution 
of  urea  nitrate,  coniine,  nicotine,  saponine, 
convolvuline,  jalappine,  and  colophonium 
•dissolved  in  KOH+Aq  do  not  ppt.  SiO2. 
(Fluckinger,  Arch.  Pharm.  (2)  144.  97.) 

Alcohol  ppts.  water  glass  as  such  from  its 
aqueous  solution,  even  when  this  is  very  dil., 
but  there  is  some  decomposition,  the  alcohol 
tending  to  hold  in  solution  a  portion  of  a 
silicate  more  alkaline  than  that  previously 
dissolved  in  H2O,  while  the  ppt.  formed  con- 
tains more  SiO2  than  the  original  silicate. 

Many  neutral  K  or  Na  salts  ppt.  water 
glass  as  such  when  added  to  aqueous  solutions. 
Like  alcohol,  these  solutions  exert  a  decom- 
posing action,  the  ppt.  being  always  more 
siliceous  than  the  original  silicate.  Na  sili- 
cate yields  a  larger  deposit  than  K  silicate; 
when  a  silicate  of  one  base  is  pptd.  by  a  salt 
of  the  other,  both  bases  enter  into  the  com- 
position of  the  ppt,  and  the  relative  propor- 
tion of  Na  and  K  is  very  nearly  the  same  as  in 
the  average  of  the  liquids  mixed. 

Different  salts  have  very  unequal  pptg. 
power,  the  acetates  and  chlorides  being  parti- 
cularly efficient.  Heat  increases  the  pptg. 
power  of  the  chlorides,  sulphates,  and  ni- 
trates, and  diminishes  that  of  the  acetates. 
The  alkali  acetates  are  somewhat  more 
efficient  than  the  chlorides,  but  NaC2H3O2 
gives  only  a  slight  ppt.  with  Na2O,  2^SiO2, 
even  after  some  time. 

NaNO8  has  but  little  effect  on  the  more 
alkaline  silicates. 

Na2SO4  has  still  less  power  than  NaNO3. 

Na2CO3  has  no  pptg.  power,  and  Na3AsO4 
or  Na3PO4  have  very  little  effect. 


MHSO4,  MHCO3,  M2HPO4,  M2HAs04 
ppt.  SiO2.  NH4  salts  also  have  that  effect. 

Pptd.  water  glass,  as  mentioned  above,  is 
much  more  sol.  in  H2O  than  ordinary  water 
glass,  and  dissolves  in  H2O  without  decomp. 
For  numerous  further  details,  see  articles  by 
Ordway  in  Sill.  Am.  J.  Sci.  vols.  32  and  33; 
also  Storer's  Diet. 

Sp.  gr.  of  water  glass  solution  containing 
14-15%  SiO2,  13-14%  Na2O,  and  70-72% 
H2O  is  1.30-1.35.  (Hager,  Comm.  1883.) 

Sp.  gr.  of  sat.  Na2SiO3+Aq  freshly  pre- 
pared at  18°  is  1,2600,  and  1  litre  contains  4.5 
gramme-equivalents  ^2Na2SiO3. 

Sp.  gr.  of  sat.  solution  of  Na2O,  3.4SiO2  is 
1.366,  and  1  litre  contains  3.7  gramme- 
equivalents  H(Na2O,  3.4SiO2).  (Kohl- 
rausch,  Z.  phys.  Ch.  12.  773.) 

Sodium  zirconium  silicate,  Na2O,  ZrO2,  SiO2. 

Decomp.  by  hot  H2O  or  HCl+Aq.  (Gibbs, 
Pogg.  71.  559.) 

Na2O,  8ZrO2,  SiO2  +  llH2O.  Decomp.  by 
H2SO4.  (Melliss.) 

Strontium  silicate,  SrSiO3. 

(Stein,  Z.  anorg.  1907,  55.  164.) 

+H2O.  Sol.  in  H2O.  (Jordis  and  Kanter, 
Z.  anorg.  1903,  35.  90.) 

Sr2SiO4.    (Stein,  Z.  anorg.  1907,  55.  167.) 

3SrO,  SiO2.  SI.  sol.' in  H2O.  Sol.  in  acids. 
(Vauquelin.) 

Thallous  silicate,  3T12O,  10SiO2. 

100  pts.  of  a  solution  of  T12O  dissolve  4.17 
pts.  SiO2  by  24  hours'  boiling.  Sol.  in  H2O. 
(Flemming,  J.  B.  1868.  251.) 

Thorium  silicate,  ThO2,  SiO2. 

Insol.  in  acids.  Attacked  by  KHSO4. 
(Troost  and  Ouvrard,  C.  R.  105.  255.) 

+  13/£H2O.  Min.  Thorite.  Decomp.  by 
HCl+Aq. 

ThO2,  2SiO2.  Insol.  in  acids  or  KHSO4. 
(T.  and  O.) 

Yttrium  silicate,  Y2O3,  SiO2. 

Attacked  by  HC1,  HNO3,  or  H2SO4+Aq. 
(Duboin,  C.  R.  107.  99.) 

Zinc  silicate,  ZnSiO3. 

(Stein,  Z.  anorg.  1907,  55.  165.) 

Zn2SiO^.  Min.  Willemite.  Gelatinizes 
with  HCl+Aq;  sol.  in  KOH+Aq. 

Decomp.  by  cold  sat.  citric  acid+Aq. 
(Bolton,  C.  N.  1881,  43.  34.) 

+H2O.  Min.  Calamine.  Sol.  in  HCl+Aq 
with  separation  of  gelatinous  SiO2,  o:H2O. 
Sol.  in  HC2H3O2+Aq,  and  KOH+Aq. 

Insol.    in    NH4OH  +  (NH4)2CO3+Aq. 
(Brandhorst,  Zeit.  angew.  Ch.  1904,  17.  513.) 

ZnO,  3SiO2.  (Borntrager,  Ch.  Z.  1893,  8. 
186.) 


810 


SILICATE,  ZIRCONIUM 


Zirconium  silicate,  SiO2,  ZrO2. 

Min.  7ircon.  Insol.  in  acids,  except  H2SO4, 
in  which  it  is  very  slowly  and  si.  sol. 

3SiO2,  2ZrO2     Min.  Auerbachite. 

"  Silicium  oxide,"  Si3H2O5. 

(Geuther,  J.  pr.  95.  430.)  This  substance 
is  identical  with  silicoformic  anhydride  ac- 
cording to  Otto-Graham's  Handb.  anorgan. 
Chem.  7te  Aufl.  2.  953. 

Siliciuretted  hydrogen. 
See  Silicon  hydride. 

Silicobromoform,  HSiBr3. 
Fumes  on  air;  decomp.  by  H2O. 

Silicochloroform,  HSiCl3. 

Decomp.  by  H2O  and  alcohol. 

Completely  miscible  with  CS2,  CC14,  CHC13, 
C6Hf,  SiCl4,  SnCl4,  TiCl4,  and  AsCl3.  (Ruff, 
B.  1905,  38.  2230.) 

Silicoethane. 
See  Silicon  hydride. 

Silicofluoroform,  SiHF3. 

Decomp.  by  H2O.  Decomp.  by  NaOH 
and  abs.  alcohol  with  evolution  of  hydrogen. 
Decomp.  by  abs.  ether.  Sol.  in  toluene. 
(Ruff,  B.  1905,  38.  63.) 

Silicoformic  anhydride, 

H2Si2O3  =  (HSiO)2O. 

Somewhat  sol.  in  H2O.  Acids,  even  cone. 
HNO3+Aq,  have  no  action,  except  HF,  which 
dissolves  it  easily  with  evolution  of  hydrogen. 
Solutions  of  alkali  hydrates,  ammonium  hy- 
drate, and  alkali  carbonates +Aq  also  dis- 
solve with  evolution  of  hydrogen.  (Ruff  and 
Wohler,  A.  104.  101.) 

Silicoiodoform,  HSiI3. 

Decomp.  by  H2O.  Sol.  in  CS2.  (Friedel, 
A.  149.  96.) 

Miscible  with  C6H6  and  CS2.  (Ruff,  B. 
1908,  41.  3739.) 

Silicomethane,  SiH4. 
See  Silicon  hydride. 

Silicomethyl  chloride,  SiH3Cl. 

Decomp.  by  H2O  and  by  alkalies.  (Besson 
and  Fournier,  C.  R.  1909,  148.  556.) 

Silicomethylene  chloride,  SiH2Cl2. 

Decomp.  by  H2O  and  by  alkalies.  (Besson 
and  Fournier,  C.  R.  1909,  148.  556.) 

Silicomolybdic  acid,  SiO2,  12MoO3  + 

26H2O. 

Very  easily  sol.  in  H2O  and  dil.  acids. 
(Parmentier,  C.  R.  94.  213.) 


Forms  a  solution  with  a  little  ether,  which 
separates  into  two  layers  by  addition  of  H2O 
or  more  ether.  (Parmentier,  C.  R.  104.  686.) 
(Copaux,  Bull.  Soc.  Min.  1906,  29.  79.) 

+32H2O.  Decomp.  by  alkali.  (Asch,  Z. 
anorg.  1901,  28.  293.) 

+33H2O.  (Copaux,  Bull.  Soc.  Min.  1906, 
29.  79.) 

Aluminum   silicomolybdate,   2A12O3,    3(SiO2, 

12MoO3)+93H2O. 
(Copaux,  A.  ch.  1906,  (8)  7.  118.) 

Aluminum  sodium  silicomolybdate,  4(Na2O, 

A12O3,  2SiO2),  Na2MoO4+7H2O. 
Sol.   in   HCl+Aq.      (Thugutt,    Z.    anorg. 
1892,  2.  87.) 

Ammonium  silicomolybdate. 

Sol.  in  H2O.    (Parmentier,  C.  R.  94.  213.) 

Barium  silicomolybdate,  2BaO,  SiO2,  12MoO3 
+  16H2O. 

(Copaux,  A.  ch.  1906,  (8)  7.  118.) 

+22H2O.  Sol.  in  4  pts.  H2O.  (Copaux, 
Bull.  Soc.  Min.  1906,  29.  80.) 

+24H2O.  Efflorescent.  Very  sol.  in  H2O. 
(Asch,  Z.  anorg.  1901,  28.  282.) 

+29H2O.  Efflorescent.  (Copaux,  A.  ch. 
1906,  (8)  7.  118.) 

Cadmium  silicomolybdate,  2CdO,  SiO2, 

12MoO3+22H2O. 

Very  unusually  sol.  in  H2O.  (Copaux,  A. 
ch.  1906,  (8)  7.  140.) 

Caesium  silicomolybdate. 

SI.  sol.  in  H2O;  insol.  in  silicomolybdic 
acid+Aq. 

Calcium  silicomolybdate,  2CaO,  SiO2, 
12MoO3+24H2O. 

Efflorescent.  Very  sol.  in  H2O.  (Asch, 
Z.  anorg.  1901,  28.  282.) 

+26H2O.  (Copaux,  A.  ch.  1906,  (8)  7. 118.) 

+31H2O.    (Copaux.) 

Chromium  silicomolybdate,  2Cr2O3,  3(SiO2, 
12MoO3)+93H2O. 

(Copaux.) 

Cupric  silicomolybdate,  2CuO,  SiO2,  12MoO3 

+31H2O.    ' 
Very  sol.  in  H2O.    (Copaux.) 

Lithium  silicomolybdate,  2Li2O,  SiO2,  12MoO3 

+29H2O. 
Very  sol.  in  H2O.    (Copaux.) 

Magnesium  silicomolybdate,  2MgO,  SiO2, 
12MoO3+30H2O. 

(Asch,  Z.  anorg.  1901,  28.  282.) 

+31H2O.  Very  efflorescent  and  sol.  in 
H2O.  (Copaux.) 


SILICON  BROMOSULPHIDE 


811 


Potassium  silicomolybdate,  2K2O,  Si02, 

12MoO3  +  16H2O. 
Efflorescent.    Very  sol.  in  H2O.     (Asch,  Z 

anorg.  1901,  28.  282.) 

1.5'K2O,  SiO2,  12MoO3  +  14H2O.     (Asch.) 
Sol.  in  H2O  with  decomp.    (Copaux.) 

Potassium      silver      silicomolybdate,      K2O 
3Ag2O,    2(Si02,     12MoO3)  +  14H2O; 
+22H2O;  +30H2O. 

Sol.  in  H2O  with  decomp.  Sol.  unchangec 
in  dil.  mother  liquor.  (Copaux,  Bull.  Soc 
Min.  1907,  30.  293.) 

Rubidium  silicomolybdate. 
SI.  sol.  in  H2O. 

Silver    silicomolybdate,    l.oAgjO,    SiO2, 
12MoO3  +  llH2O. 

Sol.  in  cold  H2O.    (Asch.) 

2Ag2O,  SiO2,  12MoO3  +  12H2O.  Decomp. 
by  boiling  H2O.  Sol.  in  NH4OH+Aq. 

4Ag2O,  SiO2,  12MoO3  +  15H2O.     (Asch.) 

Sodium   siHcomolybdate,   2Na2O,    SiO2, 
12MoO3  +  14H2O. 

(Copaux.) 

2Na2O,  SiO2,  12MoO3+21H2O.  Very  sol. 
in  H2O.  Efflorescent.  (Asch.) 

+22H2O.    (Copaux.) 

1.5Na2O,  SiO2,  12MoO3  +  17H2O.     (Asch.) 

3Na2O,  2(SiO2,  12MoO3)  +  17H2O.  (Co- 
paux.) 

Strontium  silicomolybdate,  2SrO,   SiO2, 

12MoO3+26H2O. 
(Copaux.) 

Zinc  siHcomolybdate,  2ZnO,  SiO2,  12MoO3  + 

31H2O. 
Extremely  sol.  in  H2O.    (Copaux.) 

Silicon,  Si. 

Amorphous.  Insol.  in  H2O.  Sol.  before 
igniting  in  cold  HF.  Insol.  in  other  mineral 
acids  and  aqua  regia.  Sol.  in  cone.  KOH+Aq. 
When  amorphous  Si  is  ignited,  it  becomes 
insol.  in  HF  and  KOH+Aq. 

Amorphous  Si  is  sol.  in  aqua  regia  and  in 
a  mixture  of  HNO3  and  HF.  (Vigouroux- 
Moissan,  C.  R.  1895,  120.  367.) 

Insol.  in  liquid  CO2.  (Buchner,  Z.  phys. 
Ch.  1906,  64.  674.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  830.) 

Graphitic.  Sol.  in  HNO3+HF.  (Ber- 
zelius,  A.  49.  247.) 

Crystalline.  Insol.  in  all  acids,  except  a 
mixture  of  HF  and  HNO3.  Sol.  in  moderately 
cone.  KOH+Aq  even  when  cold.  (Deville.) 

Although  it  has  been  generally  understood 
that  crystallized  Si  is  not  attacked  by  HF, 
it  is  now  found  that  this  applies  only  to  HF  + 


Aq.  Gaseous  HF  readily  attacks  cryst.  Si. 
(Newth,  C.  N.  1896,  72.  287.) 

Si  cryst.  from  Ag  is  incompletely  sol.  in 
HF.  According  to  the  temp,  to  which  the 
Ag  Si  mixture  has  been  heated,  the  following 
percentages  of  Si  are  dissolved  in  HF:  970°, 
58.02%;  1150°,  27.66%;  1250°,  19%;  1470°, 
16%.  (Moissan  and  Siemens,  C.  R.  1904, 
138.  657,  1300.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  830.) 

Silicon  amide,  Si(NH2)4. 

Unstable;  decomp.  by  H2O  and  partially 
decomp.  by  HNO3;  sol.  in  most  organic  sol- 
vents. (Lengfeld,  Am.  Ch.  J.-1899,  21.  531.) 

Decomp.  by  H2O;  insol.  in  liquid  NH3. 
(Vigouroux,  C.  R.  1903,  136.  1670.) 

Silicon  2nT>oride,  SiB3. 

Slowly  attacked  by  HNO3.  Decomp.  by 
hot  cone.  H2SO4  or  fused  KOH.  (Moissan, 
C.  R.  1900,  131.  142.) 

Silicon  Aezaboride,  SiB6. 

Readily  attacked  by  HNO3.  Slowly  de- 
comp. by  hot  cone.  H2SO4.  Not  attacked  by 
fused  KOH.  (Moissan,  C.  R.  1900,  131.  142.) 

Silicon  fnbromide,  Si2Br6. 

Decomp.  by  KOH+Aq.  (Friedel  and 
Ladenburg,  A.  203.  253.) 

HSiBr3.    See  Silicobromoform. 

Silicon  fefrabromide,  SiBr4. 

Rapidly  decomp.  by  H2O;  decomp,  in  sev- 
eral days  by  H2SO4.  (Friedel  and  Ladenburg. 

A.  147.  362.) 

Silicon  bromide,  Si3Br8. 

(Besson,  C.  R.  1910,  151.  1056.) 
Si4Brio.    (Besson.) 

Disilicon  hydrogen  pentobrcmide,  HSi2Br5  or 

Si2Br5  (?). 
Decomp.  by  H2O.    (Mahn,  Zeit.  Chem.  (2) 

.  279.) 

Silicon   teirabromide  ammonia,  SiBr4,  6NH3. 
Decomp.  by  H2O.    (Lay,  Dissert.  1910.) 
SiBr4,  7NH3.    Decomp.  by  H2O.    (Besson, 
.  R.  110.  240.) 

Silicon  bromoiodide,  SiIBr3. 
Decomp.  by  H2O.    Sol.  in  CS2.     (Friedel, 

B.  2.  60.) 

SiBr2I2.    As  above.    (F.) 
SiBrls.    As  above.    (F.) 

ilicon  bromosulphide,  SiSBr2. 
Decomp.  in  moist  air.     Violently  decomp. 
>y  H2O.    Sol.  in  CS2  and  other  organic  sol- 
ents.    (Blix,  B.  1903,  36.  4218.) 


812 


SILICON  CARBIDE 


Silicon  carbide,  SiC. 

Very  stable;  insol.  in  H2SO4  and  HNO3; 
sol.  in  fused  KOH  at  red  heat.  (Moissan, 
Bull.  Soc.  1894,  (3)  11.  997.) 

Cryst.  modification.  Insol.  in  acids;  sol. 
in  fussd  alkalies.  (Moissan,  C.  R.  1893,  117. 
427.) 

Insol.  in  all  acids;  sol.  in  molten  alkalies. 
(Muhlhaeuser,  Z.  anorg.  1894,  5.  116.) 

See  Silundum. 

Silicon  sw&chloride,  SiCl2  (?). 

Decomp.  by  H2O.  (Troost  and  Haute- 
feuille,  A.  ch.  (5)  7.  463.) 

Silicon  inchloride,  Si2C6. 

Decomp.  by  H2O  and  alkalies.  (Troost  and 
Hautefeuille,  A.  ch.  (5)  7.  459.) 

SiHCl3.    See  Silicochloroform. 

Silicon  teZrachloride,  SiCl4. 
Decomp.  by  H2O  and  alcohol. 

Silicon  ociochloride,  Si3Cls. 

"Perchlorsilicopropane."  Decomp.  by  H2O. 
(Gattermann,  B.  1894,  27.  1947.) 

Silicon  chloride,  Si4Clio. 

(Besson,  C.  R.  1909,  149.  36.) 

SisCla.  "Perchlorsilicobutane."  Decomp. 
by  H2O.  Fumes  in  the  air.  (Besson.) 

Si6Cli4.  "Perchlorsilicohexane."  Decomp. 
by  H20.  (Besson,  C.  R.  1909,  148.  841.) 

Silicon  Znchloride  ammonia,  Si2Cl6,  5NH3. 

Slowly  decomp.  by  H2O.  (Besson,  C.  R. 
110.  516.) 

Silicon  tefrachloride  ammonia,  SiCl4,  6NH3. 
Decomp.  by  H2O.    (Persoz,  A.  ch.  44.  319.) 

Silicon  tefrachloride  hydrazine,  SiCl4,  4N2H4. 
Extremely    hygroscopic    and    quickly    de- 
comp. by  H2O.    (Lay,  Dissert.  1910.) 

Silicon  chlorobromide,  SiCl3Br. 

Decomp.  by  H2O.  (Friedel  and  Laden- 
burg,  A.  145.  187.) 

SiCl2Br2.  As  above.  (Friedel  and  Laden- 
burg.) 

SiBraCl.  Decomp.  by  H2O.  (Reynolds, 
Chem.  Soc.  61.  590.) 

Silicon    chlorobromide    ammonia,    2SiCl3Br, 

11NH3. 

Decomp.  by  H2O.    (Besson,  C.  R.  112.  788.) 
SiCl2Br2,  5NH3.    As  above.    (B.) 
2SiClBr3,  11NH3.    As  above.    (B.) 

Silicon  chlorohydrosulphide,  SiCl3SH. 

Decomp.  by  H2O  or  alcohol.  (Pierre,  A.  ch. 
(3)  24.  286.) 


Silicon  chloroiodide,  SiCl3I. 

Decomp.  by  H2O.    (Besson,  C.  R.  112.  611.) 
SiCl2I2.    As  above.    (B.) 
SiClIs.    As  above.    (B.) 

Silver  chloroiodide  ammonia,  2SiCl3I,  11NH3. 

(Besson.) 

SiCl2I2,  5NH8. 

Silicon  chloronitride,  Si5N6Cl2. 
(Schiitzenberger,  C.  R.  92.  1508.) 

Silicon  chloiosulphide,  Si2Cl2S2. 

Decomp.  violently  by  H2O.  Sol.  in  CC1<. 
(Besson,  C.  R.  113.  1040.) 

SiSCl2.  Violently  decomp.  by  H2O;  sol.  in 
CS2.  (Blix,  B.  1903,  36.  4223.) 

Silicon  difluoride,  SiF2(?). 

Decomp.  by  H2O  or  NH4OH  +Aq.  (Troost 
and  Hautefeuille,  A.  ch.  (5)  7.  464.) 

Silicon  tefrafluoride,  SiF4. 

Abundantly  absorbed  by  H2O  with  decomp. 

100  pts.  H2O  absorb  140.6  pts.  SiF4  in  24 
hours  (Berzelius);  124.1  pts.  SiF4  in  24  hours 
(Davy). 

Absorbed  abundantly  by  HNO3+Aq. 
(Kuhlmann,  A.  39.  319.) 

Absorbed  abundantly  by  alcohol,  without 
separation  of  silicic  acid,  if  the  alcohol  con- 
tains less  than  8%  of  water. 

Sol.  in  cone.  HF+Aq.  Absorbed  by  ether. 
SI.  sol.  in  naptha,  and  oil  of  turpentine. 

Silicon  hydrogen  fluoride,  H2SiF6. 
See  Fluosilicic  acid. 

Silicon  fluoride  with  MF. 
See  Fluosilicate,  M. 

Silicon  fluoride  ammonia,  SiF4,  2NH3. 
Decomp.  by  H2O.     (Davy.) 

Silicon  hydride,  SiH4. 

Insol.  in  H2O.  Decomp.  by  KOH+Aq. 
Not  changed  by  NH4OH+Aq,  H2SO4+Aq, 
or  HCl+Aq. 

Si2H2.     "  Silicoacetylene." 

Sol.  in  20%  NaOH+Aq.  with  evolution 
of  H.  (Bradlev,  C.  N.  1900,  82.  149.) 

Si2H6.  "Silicoethane."  (Lebeau,  C.  R. 
1909,  148.  44.) 

SI.  sol.  in  H2O.  Best  solvent  is  ethyl 
orthosilicate.  (Moissan,  Bull.  Soc.  1903, 
(2)  29.  443.) 

Silicon  nitrogen  hydride,  SiHN. 

Decomp.  by  H2O  and  NaOH.  (Ruff,  B. 
1905,  38.  2241.) 


SILICON  OXIDE 


813 


Silicon  hydroxide,  SiO2,  #H2O. 
See   Silicic   acid. 
Si2H2O4.    See  Silicooxalic  acid. 
Si2H2O3.    See  Silicoformic  anhydride. 
Si4H4O3.    See  Silicone. 

Silicon  imide,  (Si(NH)2. 

Decomp.  by  H2O.  (Vigouroux,  C.  R. 
1903,  136.  1671.) 

SiliconeMmide,  Si(NH),. 

Decomp.  by  H2O  with  evolution  of  much 
heat.  (Blix,  B.  1903,  36.  4224.) 

Silicon  imide  hydrochloride,  Si(NH2)2,  2HC1. 
Rather  stable  in  air.     (Blix,  B.  1903,  36. 

4225.) 

Silicon  cfoiodide,  SiI2. 

Insol.  in  CS2,  CHC13,  C6H6,  and  SiCl4. 
(Friedel  and  Ladenburg,  A.  203.  247.) 

Silicon  tfniodide,  Si2I6. 

Decomp.  with  H2O  even  at  0°. 

100  pts.  CS2  dissolve  19  pts.  Si2I6  at  19°; 
26  pts.  Si2I6  at  27°.  (Friedel  and  Ladenburg, 
Bull.  Soc.  (2)  12.  92.) 

HSiI3.    See  Silicoiodoform. 

Silicon  teZraiodide,  SiI4. 

Decomp.  by  H2O.  Acts  on  alcohol  and 
ether. 

1  pt.  CS2  dissolves  2.2  pts.  SiI4  at  27° 
(Friedel,  A.  149.  96.) 

Silicon  nitride,  SiN. 

Partially  decomp.  by  boiling  with  cone 
H2SO4. 

Not  attacked  by  dil.  acids  with  the  excep- 
tion of  HF.  Decomp.  by  HF. 

Partially  decomp.  by  boiling  with  alkalies  + 
Aq.  (Weiss,  Z.  anorg.  1910,  65.  89.) 

Si2N3.  Partially  decomp.  by  boiling  with 
cone.  H2SO4. 

Not  attacked  by  dil.  acids  with  the  ex 
ception  of  HF.  Decomp.  by  HF. 

Partially  decomp.  by  boiling  with  alkalies + 
Aq.  (Weiss,  Z.  anorg.  1910,  65.  89.) 

Si3N4.    Not  attacked  by  H2O. 

Partially  decomp.  by  boiling  with   co 
H2SO4. 

Not  attacked  by  dil.  acids  with  the  excep 
tion  of  HF.  Decomp.  by  HF. 

Partially  decomp.  by  boiling  with  alkalies + 
Aq.  (Weiss,  Z.  anorg.  1910,  65.  89.) 

Silicon  nitrimide,  Si2N3H. 

"Silicam." 

Sol.  in  HF,  and  rapidly  in  KOH+Ao 
(Schutzenberger,  C.  R.  92.  1508.) 

Decomp.  by  cold,  more  rapidly  by  hot  H2C 
and  much  more  rapidly  by  alkalies.  Sol.  ir 
HF+Aq.  Not  attacked  by  HNO3.  Decomp 
by  cone.  H2SO4.  (Lay,  Dissert.  1910.) 


Not  decomposed  by  H2O. 
Sol.    in    hot    alkalies+Aq   with    decomp. 
Blix,  B.  1903,  36.  4227.) 

ilicon  sw&oxide,  Si3O2. 
(Honigschmid,  M.  1909,  30.  509.) 

silicon  monoxide,  SiO. 

Much  less  easily  sol.  in  HF+Aq  but  more 
asily  sol.  in  alkalies+Aq  than  SiO2.  (Potter, 
:.  C.  1907,  II.  1952.) 

Silicon  dioxide,  SiO2. 
See  also  Silicic  acid. 

(a)  Crystalline.     Mm.    Quartz,    Tridymite. 
Insol.  in  H2O,  and  acids,  except  HF. 

SI.  sol.  in  boiling  K2CO3+Aq,  and  KOH  + 

i;  see  below. 

Insol.  in  cold  KOH+Aq;  extremely  slowly 
sol.  in  boiling  KOH+Aq.  (Fuchs.) 

Sol.  in  HF  with  formation  of  SiF,  and  H2O. 

Insol.  in  sugar +Aq,  contrary  to  assertion 
of  Verdeil  and  Rissler.  (Petzholdt,  J.  pr. 
60.  368.) 

(b)  Amorphous.     Min.  Opal,  etc. 
Insol.  in  H2O,  and  acids  except  HF. 

100  pts.  H2O  containing  CO2  dissolve 
0.078  pt.  amorphous  SiO2  (Maschke);  0.0136 
pt.  (Struckmann). 

100  pts.  cold  HCl+Aq  of  1.088  sp.  gr.  dis- 
solve 0.017  pt.  SiO2.  (Struckmann.)  100 
pts.  HCl+Aq  of  1.115  sp.  gr.  dissolve  in  the 
cold  0.009  pt.  SiO2,  and  0.018  pt.  on  boiling. 
100  pts.  NH4OH+Aq  (containing  10%  NH8) 
dissolve  0.017  pt.  quartz  and  0.38  pt.  ignited 
SiO2.  (Pribram,  Z.  anal.  6.  119.) 

Sol.  in  boiling  K2CO3  or  Na2CO3+Aq, 
separating  out  on  cooling  as  a  gelatinous 
mass.  (Pfaff,  Schw.  J.  29.  383.)  The  differ- 
ent forms  of  SiO2  have  different  degrees  of 
solubilitv  in  K2CO3+Aq.  Unignited  amor- 
phous SiO2  from  SiF4  dissolves  most  readily, 
then  come  opal,  ignited  amorphous  SiO2, 
fused  SiO2,  and  tridymite;  quartz  powder  is 
the  most  difficultly  soluble.  (Rose.)  A 
similar  behaviour  is  shown  to  KOH+Aq. 

Opal  is  much  more  sol.  in  KOH+Aq  than 
quartz,  and  hyalite  is  the  least  sol.  of  the 
varieties  of  opal.  (Fuchs.) 

Opal  is  easily  sol.  in  KOH+Aq,  even  after 
ignition.  (Schaffgotsch,  Pogg.  68.  147.) 

Rammelsberg  (Pogg.  112.  177)  made  the 
following  experiments  on  the  solubilitv  of 
SiO2  in  KOH  +  Aq.  The  KOH + Aq  used~con- 
tained  1  pt.  KOH  to  3  pts.  H2O.  1  pt.  of 
the  powdered  mineral  was  boiled  half  an  hour 
in  a  silver  dish  with  such  an  amount  of  the 
KOH+Aq  that  20  pts.  KOH  were  present. 

7.75%  of  milky  white  quartz  was  dissolved 
by  repeating  the  above  process  three  times. 

12.8-15%  of  gray  hornstone  was  dissolved 
by  twice  boiling;  2.43%  of  moderately  finely 
powdered  agate  of  2.661  sp.  gr.  was  dissolved 
by  once  boiling;  9.7%  of  unignited  hyalite 
remained  undissolved  after  thrice  boiling; 


814 


SILICON  THORIUM  OXIDE 


21%  of  ignited  hyalite  remained  undissolved 
after  thrice  boiling;  7.21%  of  semi-opal  of 
2.101  sp.  gr.  remained  undissolved  after 
thrice  boiling;  18.5-19.2%  of  impure  semi- 
opal  of  2.101  sp.  gr.  remained  undissolved 
after  thrice  boiling;  79.9%  of  chalcedony  of 

2.624  sp.    gr.    remained    undissolved    after 
thrice  boiling;  6.12%  of  chalcedony  of  2.567 
sp.    gr.    remained   undissolved   after   fourth 
boiling;    14.4%    chrysophrase   of   2.623    sp. 
gr.  remained  undissolved  after  once  boiling; 
49.41%  of  chrysophrase  of  2.635  sp.  gr.  re- 
mained   undissolved    after    thrice    boiling; 
6.62%  of  flint  of  2.603  sp.  gr.  remained  un- 
dissolved after  twice  boiling;  38.1%  of  fire- 
opal    of  2.625  sp.  gr.  remained  undissolved 
after  fourth  boiling;  26.6%   of  fire-opal  of 

2.625  sp.    gr.    remained    undissolved    after 
fifth  boiling. 

Insol.  in  liquid  CO2.  (Biichner,  Z.  phys. 
Ch.  1908,  54.  674.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329.) 

The  solubility  of  crystals  of  quartz  on 
different  faces  in  HF  has  been  determined 
by  Lebrun.  (Belg.  Acad.  Bull.  1913,  953.) 

Silicon  thorium  oxide. 
See  Silicate,  thorium. 

Silicon  zirconium  oxide. 
.See  Silicate,  zirconium. 

Silicon  oxychloride,  Si2OCl6. 

Decomp.  by  H20  and  alcohol.     Miscible 

with    CS2,    SiCl4,    CC14,    CHC13,    or    ether. 

(Friedel  and  Ladenburg,  A.  147.  355.) 
Si403Cl10;  Si404Cl8;  Si8O1(JCl12;  (Si, 
Si4O7Cl2.  Sol.  in  above  oxy  chlorides. 

(Troost  and  Hautefeuille,  Bull.  Soc.  (2)  36. 

360.) 

OH 
Silicon  oxyfluorhydrin,  Si2O3F 

(Landolt,  A.  Suppl.  4.  27.) 

Silicon  selenide,  SiSe2. 

Decomp.  by  H2O  or  KOH  +  Aq.  (Sabatier, 
C.  R.  113.  132.) 

Silicon  sulphide,  SiS2. 

Sol.  in  H2O  with  decomp.  Acts  on  alcohol 
or  ether  in  the  cold.  (Fremy,  A.  ch.  (3)  38. 
314.) 

SiS.  Decomp.  by  H2O;  easily  sol.  in  dil. 
alkalies.  (Schiitzenberger,  Bull.  Soc.  (2)  38. 
56.) 

Silicon  sulphocfa'amide,  SiS(NH2)2. 

Slowly  decomp.  in  the  air.  Insol.  in  cold 
liquid  NH3.  (Blix,  B.  1903,  36.  4219.) 

Silicon  sulphobromide. 
See  Silicon  bromosulphide. 


Silicon  sulphochloride. 
See  Silicon  chlorosulphide. 

Silicon  sulphourea,  SiS(NH2)2. 

Slowly  decomp.  in  air. 

Decomp.  by  H2O. 

Insol.  in  cold  liquid  NH3.  (Blix,  B.  1903, 
36.  4219.) 

Silicone,  Si4H403. 

Insol.  in  H2O,  but  gives  off  hydrogen  when 
warmed  therewith.  Not  attacked  by  chlorine 
or  nitric  or  sulphuric  acids  even  on  heating, 
but  is  gradually  sol.  in  HF.  Decomp.  by 
alkalies,  even  by  the  most  dil.  NH4OH+Aq, 
with  greatest  violence  and  evolution  of  heat 
and  hydrogen  gas.  Insol.  in  alcohol,  SiCl4, 
PC13,  or  CS2.  (Wohler,  A.  127.  257.) 

H3Si3O2.  Decomp.  by  H2O  and  by  dil. 
acids.  Violently  decomp.  by  fuming  HNO3. 
Not  attacked  by  cone.  H2SO4.  Very  slowly 
decomp.  by  cone.  HC1,  rapidly  by  alkali es-j- 
Aq  and  by  pyridine.  (Honigschmid,  M. 
1909,  30.  509.) 

Insol.  in  H2O,  alcohol.  SiCl4,  PC13,  and 
CS2.  Not  attacked  by  acids  except  HF. 
(Donath  and  Liesner,  C.  C.  1909,  II.  1707.). 

H12Sii0O8.  Scarcely  attacked  by  acids, 
but  easily  decomp.  by  hot  H2O,  NaOH+Aq 
etc.  but  not  by  NH4OH+Aq.  (Kolb,  Z. 
anorg.  1909,  64,  353.) 

H10Si1008.     (Kolb.) 

H8Si8O13.    AsH12Si10O8.     (Kolb.) 

Silicowesoxalic  acid,  Si(OH)2(SiO.OH)2. 

Insol.  in  cold  H2O,  decamp,  by  hot  H2O. 
(Gattermann,  B.  1899,  32.  1116.) 

Silicooxalic  acid,  Si2H2O4-Si2O2(OH)2. 

Decomp.  by  bases  with  evolution  of  hydro- 
gen. Takes  up  HNO3  to  form  compound, 
but  not  HC1  or  H2SO4.  (Troost  and  Haute- 
feuille, A.  ch.  (5)  7.  463.) 

Silicophosphoric  acid,  SiO2,  P2O6. 

Slowly  decomp.  by  H2O.  Unchanged  by 
alcohol.  Exists  also  in  two  modifications 
which  are  not  attacked  by  H2O.  (Haute- 
feuille and  Margottet,  C.  R.  99.  789.) 

SiO2,  2P2O5+4H2O.  Decomp.  by  moist 
air.  Sol.  in  H2O  at  0°,  but  decomp.  by  warm- 
ing to  ordinary  temp.  (Hautefeuille  and 
Margottet,  C.  R.  104.  56.) 

Calcium  silicophosphate. 
See  Phosphate  silicate,  calcium. 

Silicostannic  acid. 

Calcium  silicostannate,  Ca(Si,Sn)O3. 

Not  attacked  by  acids,  KHSO4,  or  alkalies 
+Aq.  (Bourgeois,  Bull.  Soc.  (2)  47.  297.) 


SILICOTUNGSTATE,  CADMIUM  HYDROGEN 


815 


Silicodea'tungstic  acid, 

3H2O=4H2O,  SiO2,   10WO3+3H2O. 

Sometimes  sol.  in  H2O,  but  usually  sep- 
arates out  gelatinous  silica.  (Marignac,  A. 
ch.  (4)  3.  55.) 

See  also  S&icoduodecitungstic  acid. 

Ammonium    silicodea'tungstate, 

(NH4)8W10SiO36+8H2O. 
Sol.  in  4.5  pts.  H2O  at  18°.     Very  sol.  in 
hot   H2O.      (Marignac,   A.    ch.    (4)    3.    59.) 
(NH4)6H2W10SiO36+9H2O.     (Marignac.) 

Ammonium  potassium , 

(NH4)  3K4HSiW10O36 + 15H2O. 
(Marignac.) 

Barium ,  Ba4SiW10O36+22H2O. 

Precipitate.     Insol.  in  H2O.     (Marignac.) 

Potassium    ,    K8SiWioO36  +  17H2O. 

Sol.  in  H2O.    (Marignac.) 
K4H4SiW10O36+8H2O.        Sol.      in     H2O. 
(Marignac.) 

• 

Potassium  — • — •  silicotungstate  (?), 

K8SiWuO39  +  14H2O. 
K4H4SiWnO39  +  10H2O.      (Marignac.) 

Silver  — ,  Ag8W19SiO36+3H2O. 

Not  appreciably  sol.  in  cold  H2O.  (Marig- 
nac, A.  ch.  (4)  3.  65.) 

Silicotungstic   acid    or   Stticoduodeci- 
tungstic  acid,  H8SiWi2O42. 

(H4SiWi0O4o,  according  to  Copaux.  (Bull. 
Soc.  1908,  (4)  3.  101.) 

+20H2O.  Sol.  in  H2O;  very  sol.  in  alcohol; 
behaves  with  ether  as  the  acid  with  22H2O 
(Marignac,  A.  ch.  (4)  3.  10.) 

+22H2O.     Solubility  as  acid  with  29H2O. 

100  pts.  deliquesce  with  13  pts.  ether.  To 
this  mixture  20-25  pts.  of  ether  can  be  added, 
but  a  further  quantity  no  longer  mixes  with, 
but  floats  above  the  mixture.  Ethereal  solu- 
tion is  miscible  with  H2O.  Ether  is  taken  up 
by  a  saturated  aqueous  solution  with  evolu- 
tion of  heat,  until  the  volume  has  become 
doubled;  more  ether  floats  on  the  mixture. 
By  warming  the  latter  a  liquid  separates  out 
which  forms  a  layer  between  the  two  original 
layers.  Alcoholic  solution  of  the  acid  mixes 
with  an  equal  vol.  of  ether,  but  on  adding 
more  ether  a  cone,  ethereal  solution  separates 
as  a  syrupy  layer.  (Marignac,  A.  ch.  (4)  3. 
3.  10.) 

+29H2O.  Efflorescent.  Sol.  in  H2O.  Sat- 
urated solution  at  18°  contains  1  pt.  crystal- 
lized acid  to  0.104  pt.  H2O,  and  has  2.843  sp. 
gr.  Melts  in  crystal  H2O.  Easily  sol.  in 
absolute  alcohol  and  anhydrous  ether. 

+*H2O.     (Drechsel,  B.  1887,  20.  1452.) 


Aluminum  silicotungstate,  Al4Hi2(SiWi2O42)3 
+75H2O. 

Not  deliquescent;  very  sol.  in  H2O. 
(Marignac). 

Al4(SiW1204o)3+60H20.  (Wyrouboff. 

Chem.  Soc.  1897,  72,  (2)  174.) 

+87H2O.    (Wyrouboff.) 

4-93H2O.    Very  efflorescent.    (Wyrouboff.) 

Aluminum  ammonium , 

Al4(NH4)18(SiW12043)3+75H20. 
Sol.  in  H2O.     (Marignac.) 

Ammonium    — — -,    basic,     (NH4)4SiWi2O40 

4NH4OH  +  14H2O. 
(Wyrouboff,  Chem.  Soc.  1897,  72.  (2)  174.) 

Ammonium ,  (NH4)8SiW:2O42  +  16H2O. 

Very  sol.  in  hot  H2O.  (Marignac,  A.  ch. 
(4)  3.  17.) 

(NH4)4H4SiW12O42+6H2O.  Less  soluble  in 
H2O  than  the  preceding  salt.  (Marignac.) 

(NH4)4SiW12040+8H20.  (Wyrouboff, 

Chem.  Soc.  1897,  72.  (2)  174.) 

Barium ,  Ba2H4SiW12O<2  +  14H2O. 

Sol.  in  H2O. 

+22H2O.  Gradually  efflorescent.  (Marig- 
nac.) 

Sol.  in  cold  H20, 1  :  0.7  pts.  (Copaux,  Bull. 
Soc.  Min.  1906,  29.  80.) 

Sol.  in  4  pts.  cold  H2O.  (Wyrouboff,  Bull. 
Soc.  Min.  1896,  19.  278.) 

Ba4SiWi2O42+27H2O.  Nearly  insol.  in 
cold,  si.  sol.  in  hot  H2O.  (Marignac.) 

Ba2SiWi2O40  +  16H2O.    (Wyrouboff.) 

Barium    potassium   •,    Ba2K2SiWi2O40-f- 

17H2O. 
(Wyrouboff,  Chem.  Soc.  1897,  72.  (2)  176.) 

Barium     sodium    -,     Na<.Ba3SiWi2O.-2-f- 

28H2O. 

H2O  gradually  dissolves  out  sodium  silico- 
tungstate. 

Cadmium  — ,  Cd2SiW12O40+23H2O,  and 
+27H2O. 

(Wyrouboff.) 

4CdO,  3(SiO2,  12WO3)+4H2O.  (Wyrou- 
boff.) 

Caesium ,  Cs8SiWi2O42. 

100  pts.  H2O  dissolve  only  0.005  pt.  at  20°; 
0.52  pt.  at  100°. 

Completely  insol.  in  alcohol,  and  HCl+Aq. 
Somewhat  sol.  in  dil.  NH4OH+Aq.  (Godef- 
froy,  B.  9.  1363.) 

Cadmium    hydrogen    ,     2Cd2SiWi2O40, 

H4SiW12O,0+42H2O. 
(Wyrouboff.) 


816 


SILICOTUNGSTATE,  CALCIUM 


Calcium     silicotungstate,     Ca2H4SiWi2O42 
20H2O. 

Not  deliquescent.  Extremely  easily  sol 
in  H2O.  (Marignac.) 

Ca2SiW12O40  +  18,  24  and  27H2O.  (Wyrou- 
boff.) 

Calcium  silicotungstate  nitrate,  Ca2SiWi2O40 
Ca(NO3)2  +  15H2O. 

(Wyrouboff.) 

Cerous  —  ,  Ce2SiW12O4o+27H2O. 

(Wyrouboff.) 

Ce2SiW12O4o,  CeH2SiWi2O,0-|-34H2O. 
(Wyrouboff.) 

Chromium  -  ,  Cr4(SiWi2O40)3+60,  87  and 

93H2O. 
(Wyrouboff.) 

Cupric  --  ,  Cu2SiW12O40+18,  27  and  29H2O. 
Very  efflorescent.    (Wyrouboff.) 

Didymium  -  ,  Di2SiW12O40+26  and  27H2O. 

(Wyrouboff.) 

Di2SiW120,;0,  DiH2SiW12040+34H20. 
(Wyrouboff.) 

Gallium  —  ,  Ga4(SiW12O40)3+60,  87,  and 

93H2O. 
(Wyrouboff.) 

Glucinum  -  -,  Gl4(SiW12d40)3+45,  87  and 

93H2O. 
(Wyrouboff.) 

Indium  -  ,  In2O3,  H2O,  2(SiO2,  12WO3)  + 
40H2O. 

(Wyrouboff.) 

2In2O3)  3(SiO2,  12WO3)+63  and  93H2O. 
(Wyrouboff.) 

Iron   (ferric)   -  ,   Fe4(SiW]2O40)3+60  and 

93H20. 
(Wyrouboff.) 

Lanthanum  —  ,  La2SiWi2O40+27H2O. 

Efflorescent.    (Wyrouboff.) 
La2SiWi2O.0.LaH2SiW12O40+34H2O. 
(Wyrouboff.) 

Lead  -  ,  basic,  Pb2SiW12O40,  2PbO+20H2O. 
SI.  sol.  in  H2O.    (Wyrouboff.) 

Lead  -  ,  Pb2SiWi2O40+21  H2O. 
Sol.  in  H2O.    (Wyrouboff.) 

Lithium  —  ,   Li2O,  SiO2,   12WO3  +  14  and 

24H20. 
(Wyrouboff.) 


Magnesium  —  ,  Mg2H4SiWi2O42 
Stable  on  the  air.    (Marignac.) 


Mercurous  silicotungstate,  basic, 
Hg4SiW12O40,  2Hg2O+5H2O. 
Insol.  inH2O.    Insol.  in  dil.  HNO3.    Slowly 
sol.  in  cone.  warm.  HNO3.    (Wyrouboff.) 

Mercurous  -  •,  Hg8SiWi2O42. 

Insol.  in  H2O.    Scarcely  sol.  in  dil.  HNO3  + 
Aq.    (Marignac,  A.  ch.  (4)  3.  43.) 

Mercuric  -  ,  Hg2SiW12O40  +  15H2O. 

Very  sol.  in  H2O.     Solution  decomp.  on 
boiling.    (Wyrouboff.) 

Potassium  -  ,  basic,  K4SiW12O40,  4KOH  + 

12H2O. 

1  pt.  is  sol.  in  10  pts.  H2O  at  18°.    (Wyrou- 
boff.) 


Potassium  -  ,  K8SiWi2O4 

Sol.  in  10  pts.  H2O  at  18°,  and  less  than 
3  pts.  at  100°.  (Marignac.) 

+20H2O.  Much  less  sol.  in  cold  than  hot 
H2O.  Extremely  sol.  in  hot  H2O.  More  sol. 
than  above  comp.  (Marignac.) 

K4ELSiW12O42+7H2O.  Solubility  as  pre- 
ceding salt. 

K4H4SiW12O42  +  16H2O.  Sol.  in  3  pts.  H2O 
at  20°. 

K6H:9(SiWi2O.,2)2+25H2O.  Decomp.  by 
dissolving  in  H2O.  (Marignac.) 

K4SiW12O  0+6  and  15H2O.    (Wyrouboff.) 

K4SiW12O40,  K2H2SiW]2O40-f29H2O. 
(Wyrouboff.) 

Rubidium  -  ,  Rb8SiW12O42. 

Sol.  in  145-150  pts.  H2O  at  20°  and  in  19-20 

pts.  at  100°.    Insol.  in  alcohol;  difficultly  sol. 

n  acidified,  but  extremely  easily  in  ammonia- 

cal  H2O.    (Godeffroy,  B.  9.  1363.) 
Rb2H2SiW12O40+5H2O.    (Wyrouboff.) 
Rb4SiW12O40,  Rb2H2SiWi0O40+22H2O. 

Wyrouboff.) 

Silver  -  ,  Ag4H4SiW12O42+7H2O. 

Very  si.  sol.  in  H2O;  sol.  in  dil.  HNO3  + 
Aq.  (Marignac.) 

SI.  sol.  in  H2O.    (Wyrouboff.) 

Sodium  -  ,  basic,  Na4SiW12O40,  4NaOH  + 
5H2O. 

(Wyrouboff.) 

Sodium  -  ,  Na8SiW12O42+7H2O. 

The  saturated  solution  at  19°  contains  0.21 
pt.  H2O  to  1  pt.  of  the  salt  dried  at  100°,  and 
las  sp.  gr.  =  3.05.  (Marignac.) 

Na4H4SiWi2O42  +  llH2O.    Stable  on  air. 

+  18H2O.    Efflorescent.    (Marignac.) 

Na2H6SiWi2O42  +  14H2O.  Decomp.  by  dis- 
solving in  H2O.  (Marignac.) 

Na4SiW12O40+14,  16  and  20H2O.  (Wyrou- 
>off.) 


SILVER 


817 


Sodium  silicotungstate  nitrate, 

3Na4H4SiW12Q42,  4NaNO3+39H2O. 
Slightly  deliquescent.    (Marignac.) 

Strontium  -  ,  Sr2SiW12CU+16,  17,  23  and 

27H2O. 
(Wyrouboff.) 

Thallium  --  •,  Tl2H2SiW12O40+9H2O. 
(Wyrouboff.) 

Thorium  —  —  ,  basic. 

Insol.  in  H2O.    (Wyrouboff.) 

Thorium  -  ,  Th2SiWi2O40+27H2O. 
Very  sol.  in  H2O.    (Wyrouboff.) 
Th2SiW12O40,  2H4SiW10O40+45H2O.    • 

(Wyrouboff.) 

Uranium  -  . 

Thirteen  salts  are  described  by  Wyrouboff. 

Uranyl  -  . 
Seven  salts  are  described  by  Wyrouboff. 

Zinc  --  ,  Zn2SiWi2O40+18,  27  and  29H2O. 
(Wyrouboff.) 

Silicovanadiomolybdic  acid. 

Ammonium  silicovanadiomolybdate, 

3(NH4)2O,  SiO2,  V2O5,  9MoO3+20H2O. 

Sp.  gr.  of  sat.  solution  containing  0.32016  g. 
salt  in  1  ccm.  at  18°  =  1.21322.  (Friedheim, 
B.  1900,  33.  1624.) 

3(NH4)2O,  SiO2,  V2O6,  10MoO3+21H2O. 
Sp.  gr.  of  sat.  solution  containing  0.35026  g. 
of  salt  in  1  ccm.  at  18°  =  1.25275.  (Fried- 
heim.) 

3(NH4)2O,  V2O5,  SiO2,  HMoO3+27H2O. 
Sp.  gr.  of  sat.  solution  containing  0.38086  g. 
salt  in  1  ccm.  at  18°  =  1.29266.  (Triedheim.) 

3(NH4)2O,  V2O5,  SiO2,  15MoO3+24H2O. 
Sp.  gr.  of  sat.  solution  containing  0.48997  g. 
salt  in  1  ccm.  at  18°  =  1.43761.  (Friedheim.) 

Ammonium  potassium  —  —  •  (NH4)2O,  2K2O, 

SiO2,  V2O5,  9MoO8+20H2O. 
Sp.  gr.  of  sat.  solution  containing  0.24021 
g.  salt  in  1  ccm.  at  18°  =  1.17031.     (Fried- 
heim.) 


,  2K20,  Si02,  V205,  10MoO,+ 
21H2O.  Sp.  gr.  of  sat.  solution  contain- 
ing 0.25914  g.  salt  in  1  ccm.  at  18°  =  1.19184. 
(  Friedheim.) 

(NH4)2O,    2K2O,    SiO2,    V2O5,    HMoOH- 
12H2O.     Sp.    gr.    of   sat.    solution   contain- 
ing 0.27914  g.  salt  in  1  ccm.  at  18°  =  1.21378. 
'  (Friedheim.) 

Ammonium    zinc    —  —  ,    4(NH4)2O,    2ZnO, 

2SiO2,  3V2O6,  18MoO3  +  15H2O. 
SI.  sol.  in  H2(X    (Blum,  Dissert.  1904.) 


Silicovanadiotungstic  acid. 

Ammonium  silicovanadiotungstate,  3(NH4)2O, 
SiO2,  V2O5,  9WO3+24H2O. 

Can  be  cryst.  from  H2O.  (Friedheim,  B. 
1902,  36.  3244.) 

(NH4)6SiV2W10O4o+21H2O.  1  cc.  of  sat. 
solution  in  H2O  at  17.5°  contains  0.6652  g. 
of  the  hydrated  salt.  Sp.  gr.  of  this  solution  = 
1.4505.  Decomp.  by  cone,  acid  and  alkali. 
(Friedheim.) 

Ammonium  barium  potassium , 

(NH4)2K2BaSiV2W10O40+25H2O. 
SI.  sol.  in  H2O.    Decomp.  by  cone,  acids 
and  alkalies.    (Friedheim.) 

Ammonium  potassium 

(NH,)K5SiV2W10O40+23H2O. 
1  ccm.  of  sat.  solution  at  17.5°  contains 
0.5072  g.  of  the  salt.  Sp.  gr.  of  the  solution 
at  20°  =  1.3462.  Can  be  cryst  from  H2O. 
Decomp.  by  cone,  acids  and  alkalies.  (Fried- 
heim.) 

Barium ,  Ba3SiV2W10O40-|-28H2O. 

1  ccm.  of  the  sat.  solution  in  H2O  at  17.5° 
contains  0.0384  g.  of  the  salt.  Sp.  gr.  of  the 
solution  =  1.0307.  Decomp.  by  cone,  acids 
and  alkalies.  (Friedheim,  B.  1902,  35.  3245.) 

6BaO,  2SiO2,  3V2O6,  18WO3+50H2O. 
SI.  sol.  in  H2O.  (Friedheim.) 

7BaO,  2SiO2,  3V2O6,  18WO3+83H2O. 
SI.  sol.  in  H2O.  (Friedheim.) 

Potassium ,  K6SiV2WioO4o+22H2O. 

Sol.  in  H2O.  Can  be  cryst.  from  H2O 
without  decomp.  Decomp.  by  cone,  acids 
and  alkalies.  (Friedheim.) 

6K2O,  2SiO2,  3V2O5,  18WO3+31H2O.  Sol. 
in  H2O.  (Friedheim.) 

7K2O,  2SiO2,  3V2O5,  18WO3-|-42H2O.  Sol. 
in  H2O.  (Friedheim.) 

Sodium ,  Na6SiV2WioO4o+29H2O. 

Very  sol.  in  H2O.  Decomp.  by  cone  acids 
and  alkalies.  (Friedheim.) 

Silundum,  SixCy. 

Not  attacked  by  hot  Cl  or  cone,  acids. 
(Amberg,  Z.  Elektrochem.  1909,  15.  725.) 

Silver,  Ag. 

Not  attacked  by  H2O.  Absolutely  insol.  in 
HC1  or  HC2H3O2+Aq.  (Lea,  Sill.  Am.  J. 
144.  444.)  Easily  sol.  in  HNO3+Aq  on  warm- 
ing, if  not  too  cone.  Only  a  minute  trace  is 
dissolved  in  an  hour  by  cold  dil.  HN03+Aq  (1 
pt.  HNO3+Aq  of  sp.  gr.  1.40  :  10  pts.  H2O). 
(Lea.)  Sol.  in  hot  cone.  H2SO4  with  evolution 
of  SO2.  SI.  sol.  in  dil.  H2SO4-j-Aq  (1  .  4),  but 
with  more  dil.  H2SO4+Aq  the  different  forms 
of  Ag  behave  differently.  (Lea.) 

Sol.  in  HI-fAq  at  ordinary  temperature. 


818 


SILVER  ACETYLIDE 


Sol.  in  KI+Aq  with  access  of  air.  Sol.  in  hot 
KCN+Aq.  (Christomanos,  Z.  anal.  7.  301.) 

Sol.  in  chromic,  iodic,  chloric  and  bromic 
acids.  Dil.  H2SO<-  alone  is  incapable  of  dis- 
solving finely  divided  Ag,  and  the  seeming 
solvent  action  is  due  to  the  oxygen  of  the  air, 
oxygen  dissolved  in  the  acid,  or  derived  from 
some  external  source.  (Hendrixson,  J.  Am. 
Chem.  Soc.  1903,  25.637.) 

Boiling  H2SO4  dissolves  pure  Ag  only  when 
concentration  equals  60°  B.  More  dil.  acid 
dissolves  only  the  impure  metal.  (Pannani, 
Gazz.  ch.  it.  1909,  39.  (2)  234.) 

Slowly  decomp.  into  AgCl  by  alkali  chlor- 
ides+Aq;  also  by  CuCl2,  etc.+Aq. 

Somewhat  sol.  in  NH4OH+Aq  in  presence 
of  O.  (Lea,  Sill.  Am.  J.  144.  444.) 

Sol.  in  KMnO4+dil.  H2SO4+Aq.  (Fried- 
heim,  B.  20.  2554.) 

Sol.  in  Fe2(SO4)3+Aq,  especially  on  heat- 
ing, but  completely  insol.  in  FeSO4+Aq. 
(Vogel.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  829.) 

Allotropic  forms — (a).  Very  sol.  in  H2O. 
Solution  is  pptd.  by  saline  solutions  or  almost 
any  neutral  substance.  Alkali  sulphates, 
nitrates,  and  citrates  ppt.  it  in  a  sol.  form, 
while  MgSO4,  CuSO4,  FeSO,,  NiSO4,  K2Cr2O7, 
K4Fe(CN)6,  Ba(NO3)2,  and  even  AgNO3+Aq 
ppt.  it  in  an  insol.  form,  which,  however,  may 
be  made  sol.  again  by  treatment  with  many 
substances,  as  Na2B4O7,  K2SO4,  or  Na2SO4+ 
Aq.  NaNO2+Aq  ppts.  the  Ag  from  its  solu- 
tion in  a  perfectly  insol.  form. 

(j8).  The  ppt.  from  aqueous  solution  by 
salts  is  sol.  in  NH4OH+Aa.  (Lea,  Sill.  Am. 
J.  137.  476.) 

Many  other  allotropic  forms  exist.     (Lea.) 

Pure  colloidal  silver  is  also  sol.  in  alcohol. 
Schneider,  B.  25.  1164.) 

Entirely  sol.  in  H2O,  even  when  dry. 
(Schneider,  Z.  anorg.  1894,  7.  339.) 

Silver  acetylide,  Ag2C2.  . 

Sol.  in  KCN+Aq  with  evolution  of  C2H2. 
Decomp.  by  HCl+Aq.  (Arth,  C.  R.  1897, 
124.  1535.) 

Silver  amide,  AgNH2. 

Ppt.;  sol.  in  ammonium  salts+Aq  and  in 
excess  of  potassium  amide.  Sol.  in  liquid 
NH3.  Insol.  in  Ag  salts+Aq.  (Franklin, 
J.  Am.  Chem.  Soc.  1905,  27.  833.) 

Sol.  in  excess  of  KNH2.  (Franklin,  Z 
anorg.  1905,  46.  16.) 

Silver  antimonide,  Ag2Sb  or  Ag4Sb. 

Min.     Discrasite.      Sol.     in     HNO3+Aq 
Ag3Sb.     Insol.  in  HCl+Aq;  decomp.  bj 

HNO3+Aq.    (Christofle.) 

Silver  azoimide,  AgN3. 

Insol.  in  hot  or  cold  H2O  or  dil.  acids;  sol 
in  cone,  mineral  acids.  Sol.  in  NH4OH+Aq 
(Curtius,  B.  23.  3023.) 


Silver  bromide,  AgBr. 

Insol.  in  H2O,  or  H2O  acidulated  with 
HNO3,  H2SO4,  or  HC2H3O2  between  0°  and 
33°.  If  flbcculent  or  pulverulent,  it  is  sensibly 
sol.  therein  above  33°,  but  if  granular  only 
above  50°,  and  then  very  slightly.  (Stas,  A. 
ch.  (5)  3.  289.)  Ag  can  be  detected  as  AgBr 
n  10,000,000  pts.  H2O.  (Stas.) 

Calculated  from  the  electrical  conductivity 
of  AgBr+Aq,  AgBr  is  sol.  in  1,971,658  pts. 
H2O  at  20.2°,  and  775,400  pts.  at  38°.  (Holle- 
man,  Z.  phys.  Ch.  12.  133.) 

By  same  method  Kohlrausch  and  Rose  cal- 
culate that  1  1.  H2O  dissolves  0.4  mg.  AgBr 
at  18°.  (Z.  phys.  Ch.  12.  240.) 

Solubility  in  H2O  =  0. 109  mg.  per  1.  (Prud- 
homme,  J/chim.  Phys.  9.  519.) 

Solubility  in  H2O  =  6.6  X  10~7  at  25°.  (Good- 
win, Z.  phys.  Ch.  1894,  13.  645.) 

Solubility  of  AgBr  in  H2O  at  25°  equals 
8.1  X10-7  g.  mols.  per  1.  (Thiel,  Z.  anorg. 

1900.  24.  57.) 

Aq.  solution  sat.  at  21.1°  contains  0.57  X 
10~6  gr.  equiv.  per  litre.  (Kohlrausch,  C.  C. 

1901,  II.  1299.) 

1  1.  H2O  dissolves  0.000137  g.  AgBr  at  25°. 
(Abegg  and  Cox,  Z.  phys.  Ch.  1903,  46.  11.) 

0.84  X 10  4  g.  are  dissolved  per  liter  of  sat. 
solution  at  20°.  (Bottger,  Z.  phys.  Ch.  1903, 
46.  603.) 

1  l.H2O  dissolves  0.107  mg.  AgBr  at  21°. 
(Kohlrausch,  Z.  phys.  Ch.  1904,  50.  356.) 

3.7  mg.  AgBr  are  contained  in  1  liter  of  sat. 
solution  at  100°.  (Bottger,  Z.  phys.  Ch. 
1906,  56.  93.) 

1  mg.  in  1  1.  of  sat.  solution  at  21°.  (Kohl- 
rausch, Z.  phys.  Ch.  1908,  64.  168.) 

Solubility  in  H2O=8.8XH)-7  g.  mol. 
per  litre  at  25°.  (A.  E.  Hill,  J.  Am.  Chem. 
Soc.  1908,  30.  74.) 

Boiling  H2O  dissolves  0.000003502  of  its 
weight  of  AgBr.  HNO3+Aq  (1%  HNO3) 
dissolves  0.00000543  of  its  weight  of  AgBr  at 
100°  with  si.  decomposition.  The  solution 
is  pptd.  by  AgNO3+Aq  or  HBr  (or  MBr)  + 
Aq,  but  not  completely.  I  pt.  of  AgBr  m 
solution  requires  3  pts.  of  Br  as  MBr  (or 
HBr),  or  of  Ag  as  AgNO3  in  order  to  be  wholly 
precipitated.  (Stas.) 

Not  attacked  by  boiling  HNO3+Aq;  si. 
sol.  in  cone.  HBr  or  HCl+Aq  (Lowig). 
Boiling  cone.  H2SO4  decomposes  it  (Balard), 
hardly  acts  on  it  (Dumas),  dissolves  a  small 
quantity,  which  is  repptd.  by  H2O  (Berze- 

Very  si.  sol.  in  dil.,  easily  in  cone.  NH4OH 
+Aq.  100  pts.  NH4OH+Aq  (0.986  sp.  gr.) 
dissolve  0.51  pt.  AgBr  (dried  at  100°)  at  80°, 
and  about  double  that  amount  of  freshly 
pptd.  AgBr.  (Pohl,  W.  A.  B.  41.  2670 

1  g.  freshly  pptd.  AgBr  is  sol.  in  250  ccm. 
10%  NH4OH+Aq,  but  insol.  in  an  ammoma- 
cal  solution  of  AgCl.  (Seiner,  Pharm.  J. 

T  e;S  AgBr  dissolves  in  8779.4  g.  5%  NH4OH 
+Aq  (sp.  gr.=  0.998)  at  12°,  and  in  288.5  g. 


SILVER  BROMIDE 


819 


10%    NH4OH+Aq    (sp.    gr.=0.96)    at    12°. 
(Longi,  Gazz.  ch.  it.  13.  87.) 

Solubility  of  AgBr  in  NH4OH+Aq  at  15°. 
G.  mols.  per  1. 


NH3 

AgBr 

Sp.  gr.  15.5° 

1.085 
2.365 
3.410 
4.590 
5.725 

0.0011 
0.0031 
0.0050 
0.0074 
0.0101 

0.9932 
0.9853 
0.9793 
0.9720 
0.9655 

(Bodlander,  Z.  phys.  Ch.  1892,  9.  734.) 

Solubility  in  NH4OH+Aq  at  0°. 
10  ccm.  of  the  solution  contain  g.  NH3  and 
mg.  Ag  Br. 


g.  NH3 

Mg.  AgBr 

g.  NH3 

Mg.  AgBr 

0.307 

8.0 

2.627 

106.7 

0.488 

9.6 

3.126 

156.8 

0.669 

17.2 

3.389 

198.7 

0.829 

21.2 

3.652 

266.9 

1.151 

34.9 

3.722 

288.8 

1.532 

55.7 

3.770 

293.0 

1.809 

72.2 

3.926 

289.2  ' 

1.953 

74.1 

3.995 

285.0 

(Jarry,  A.  ch.  1899,  (7)  17.  364.) 

Solubility  of  AgBr  in  NH4OH+Aq  at  25°. 
G.  mols.  per  1. 


NH3 

AgBr 

NH3 

AgBr 

0.1932 
0.3849 
0.7573 

0.00060 
0.00120 
0.00223 

1.965 
3.024 
5.244 

0.00692 
0.01163 
0.02443 

(Bodlander  and  Fittif,  1902,  Z.  phys.  Ch.  39. 
597.) 

Solubility  in  NH4OH+Aq  at  25°. 


g.  at.  Ag  per  1. 

Mols.  NH3  per  1. 

0.00170 

0.00159 
0.000941 
0.00107 
0.000391 
0.000386 
0.000276 
0.000264 

0.450 
0.497 
0.268 
0.273 
0.115 
0.118 
0.0764 
0.0777 

(Whitney  and  Melcher,  J.  Am.  Chem.  Soc. 
1903,  25.  79.) 

Sol.  in  hot  NH4Cl+Aq.  Very  si.  sol.  in 
NH4  carbonate,  sulphate,  or  succinate+Aq, 
and  still  less  in  nitrate.  (Wittstein.)  Not 
very  easily  sol.  in  Na2S2O3+Aq  when  sus- 
pended in  much  H2O,  and  is  separated  out 
again  by  KBr+Aq.  (Field,  C.  N.  3.  17.) 

Sol.  in  KCN+Aq.     SI.  sol.  in  cone.  KC1, 


KBr,  NaCl,  NaBr,  NH4C1,  or  NH4Br+Aq; 
but  insol.  when  dilute. 

Traces  only  dissolve  in  alkali  nitrates  +Aq. 
(Fresenius,  C^uant.  Anal.) 

Abundantly  sol.  in  Hg(NO3)2+Aq.  100 
ccm.  H2O  containing  10  ccm.  normal 
Hg(NO3)2+Aq  dissolve  0.0383  g.  AgBr. 
(Stas.) 

Solubility  of  AgBr  in  Hg(NO3)2+Aq  at  25°. 
G.  mols.  per  1. 


Hg(NO3)2 
HNOs 

AgBr 

Hg(N03)2 
HNO3 

AgBr 

1 

0.10 
0.05 

0.03660 
0.00873 
0.00639 

0.025 
0.0125 
0.0100 

0.00459 
0.00329 
0.00306 

HNO3  was  present  in  all  cases,  and  it  was 
found  that  there  was  no  difference  in  solubil- 
ity of  AgBr  with  concentrations  between 
0.1N  and  2N  HNO3.  Cryst.  and  amorphous 
AgBr  showed  the  same  solubility.  (Morse, 
Z.  phys.  Ch.  1902,  45.  708.) 

Difficultly  sol.  in  hot  cone.  AgNO3+Aq. 
(Risse,  A.  111.  39.) 

100  ccm.  of  a  3-N  solution  of  AgNO3  dis- 
solve 0.04  g.  AgBr  at  25°.  Much  less  sol., 
in  AgNO3+Aq  than  Agl.  (Hellwig,  Z, 
anorg.  1900,  25.  176.) 

Solubility  in  AgNO3+Aq. 


Volumetric  measurements 


AgNOa 

N/10 
KBr 
ccm. 

Opal- 
escent 
at 

G.  AgBr 
retained 
per  100  g. 
AgNOs 

c 

0.65 

22° 

0.129 

0.72 

35 

0.144 

10  g.  made  up  to 

0.8 

44 

0.159 

32  g.  per  100  g.  < 

0.9 

62 

0.178 

of  solution 

1.0 

67 

0.188 

1.1 

77 

0.207 

t 

1.2 

79 

0.226 

6.0 

37 

1.13 

8.0 

53 

1.50 

10.0 

67 

1.88 

10  g.  made  up  to 

11.25 

72 

2.12 

70  g.  per  100  g.  - 

12.0 

74 

2.26 

of  solution 

12.75 

79 

2.40 

13.5 

•82 

2.54 

15.5 

85.5 

2.92 

17.5 

90 

3.29 

Gravimetric  measurements  at  14.5° 


G.  AgNOa 

ccm.  H2O 

Strength 
of  AgNOs 

% 

G.  AgBr  re- 
tained per 
100  g.  AgNOs 

7.326 
8.290 
7.255 
7.35 

9.32 
7.65 

4.84 
3.95 

44 
52 
60 
65 

0.144 
0.185 
0.283 
0.365 

(Lowry,  Roy.  Soc.  Proc.  1914,  91.  A,  65.) 


820 


SILVER  BROMIDE 


100  g.  KBr  in  cone.  KBr+Aq  dissolve  3019 
mg.  AgBr  at  15°;  95  g.  NaCl  +  10  g.  KBr  dis- 
solve only  75  mg.  AgBr  at  15°.     (Schierholz, 
W.  A.  B.  101,  2b.  4.) 

Solubility  in  KBr+Aq  at  25°. 

Solubility  in  salts  +Aq. 

Solvent 

Cone. 

Grams 
AgBr  sol.  in 
100  grams 
solvent 

Sodium  thiosulphate 

<t              a              f. 

«               u              K 
"              •'              "         . 
it               «               « 

\  Sodium  sulphite 

U                            K 

Ammonium  sulphite 
Potassium  cyanide 
Ammonium  sulphocyanide 

(t 

\  Potassium 
Calcium 
Barium 
Aluminum 
Thiocarbamide 

Thiosinamine 

K 

u 

1 

.   5 
10 
15 
20 
10 
20 
10 
5 
5 
10 
15 
10 
10 
10 
10 
10 
1 
5 
10 

0.35] 
1.90 
3.50 
4.20 
5.80, 
0.04< 
0.08 
Trace 
6.55, 
0.2r 
2.04 
5.30 
0.73' 
0.53 
0.35 
4.50 
1.87 
0.08 
0.35 
0.72 

y20° 

•25° 

s 

20° 
>25° 

Mol.  KBr  in  1  litre 

G.  AgBr  in  1  litre 

4.864 
4.44 
4.18 
3.68 
2.81 
2.76 

26.44 

17.95 
13.50 
7.50 
2.34 
2.20 

(Hellwig,  Z.  anorg.  1900,  26.  183.) 

Sol.  in  cone.  KBr  or  NaBr+Aq  (Lowig), 
but  less  than  Agl  in  KI+Aq  (Field). 
100  g.  NaCl  in  cone.  NaCl+Aq  dissolve 
474  mg.  AgBr  at  15°;  100  g.  NaCl  in  21% 
NaCl+Aq   dissolve    188   mgr.   AgBr   at    15°. 
(Schierholz,  W.  A.  B.  101,  2b.  4.) 

Solubility  of  AgBr  in  Na2SO3+Aq  at  25°. 
G.  formula  weights  per  1. 

(Valenta,  M.  1894,  16.  250.) 

Solubility  of  AgBr  in  salts  +Aq  at  (?)°. 
(G.  AgBr  sol.  in  1  1.  of  1%  solution  of  salts.) 

NaSCN                  2.06 

Sos                    Ag 

Sos                     Ag 

0.232         0.0025 
0.406         0.0023 
0.448         0.00,23 

0.466         0.0053 
0.474         0.0055 
0.675         0.0084 

(Luther  and  Leubner,  Z.  anorg.  1912,  74.  393.) 

Solubility  of  AgBr  in  Na2SO3  at  (?)°. 
(g.  salts  per  1.  of  solution.) 


NH4SCN 

(NH4)2C03 

Na2SO4 


0.03 

0.004 

0.055 


Na2S03 

AgBr 

Na2SO3 

AgBr 

83.75 
70.75 
38.2 
17.65 
9.47 
4.85 

0.790 
0.570 
0.265 
0.116 
0.0526 
0.0329 

2.08 
1.13 
0.59 
0.3 
0.17 
0.08 

0.0159 
0.0086 
0.0045 
0.0039 
0.0022 
0.00075 

(Mees  and  Piper,  Photog,  J.  1912,  36.  234.) 
Solubility  in  Na2S2O3+Aq  at  35.° 


g.  Na2S2Os  in  1  liter 


100 
200 
300 
500 


g.  AgBr  corresponding 
to  each  g. 


0.376 
0.390 
0.397 
0.427 


(Richards  and  Faber,  Am.  Ch.  J.  1899,  21. 
169.) 

(NH4)2S2O3+Aq.  dissolves  AgBr  more 
rapidly  than  does  Na2S2O3+Aq.  (Lumie"re 
and  Seyewitz,  C.  C.  1908,  II.  1138.) 


(Mees  and  Piper,  Photog.  J.,  1912,  36.  234.) 

In  a  solution  of  NaC2H3O2+Aq,  containing 
10  ccm.  of  sat.  NaC2H3O2+Aq  at  15°  and 
20  ccm.  normal  HC2H3O2+Aq  mixed  with 
970  ccm.  H2O,  about  double  the  amt.  of  floc- 
culent  AgBr  is  dissolved  in  the  cold  that  is 
dissolved  by  boiling  H2O  from  granular  AgBr. 
This  solution  required  3  pts.  of  Ag  or  Br  to 
ppt.  the  AgBr  in  solution.  Pulverulent  or 
granular  AgBr  are  wholly  insol.  in  dil.  or 
cone,  acetates +Aq.  (Stas.) 

Sol.  in  Hg(C2H3O2)2+Aq. 

100  ccm.  H2O  containing  10%  of  normal 
Hg(C2H3O2)2+Aq  dissolves  0.0122  g.  AgBr 
at  20°.  (Schierholz.) 

Very  sol.  in  liquid  NH3.  (Franklin,  Am. 
Ch.  J.  1898,  20.  829.) 

Solubility  in  10  cc.  methylamine+Aq  of 
different  concentrations  at  11.5.° 

g.  NH2CH3     4.844      4.311      3.562      3.258 
mg.  AgBr        289          127  73  55 

g.  NH2CH3     1.797      1.513      1.317      1.101 
mg.  AgBr  28  16  12  7 

(Jarry,  A.  ch.  1899,  (7)  17.  378.) 


SILVER  CHLORIDE 


821 


Solubility  in  methylamine+Aq  at  25°. 


G.  mol.  per  1. 


CH«NH2 

AgBr 

0.02 

0.04 
0.074 
0.0947 
0.1950 

0.00026 
0.00034 
0.000395 
0.00041 
0.00045 

(Wuth,  B.  1902,  36.  2416.) 
Solubility  of  AgBr  in  methylamine+Aq  at  25°. 


G.  mol.  per  1. 


CH3NH2 
1.017 

0.508 
0.203 


AgBr 

CHsNJ 

0.0025 
0.0013 
0.00049 

o.io; 

0.051 

AgBr 


0.00026 
0.00012 


(Bodlander  and  Eberlein,  B.  1903,  36.  3948.) 
Solubility  in  ethylamine+Aq  at  25°. 


G.  mol.  per  1. 


C2H5NH2 

AgBr 

0.01272 
0.03942 
0.05512 
0.05572 
0.10300 

0.0000867 
0.000137 
0.000193 
0.000258 
0.000711 

(Wuth,  B.  1902,  35.  2416.) 

At  25°,  1  1.  ethylamine+Aq  containing 
0.483  g.  mol.  CANHa  dissolves  0.00231  g. 
mol.  AgBr;  0.200  g.  mol.  C2H5NH2,  0.0097  g. 
mol.  AgBr.  (Bodlander  and  Eberlein,  B. 
1903,  36.  3948.) 


Insol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1370.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II,  1014);  (Naumann,  B.  1904,  37.  4329.) 

Sol.  in  alcoholic  thiourea.  (Reynolds, 
Chem.  Soc.  1892,  61.  251.) 

Insol.  in  methyl  acetate.  (Bezold,  Dissert. 
1906);  (Naumann,  B.  1909,  42.  3790.)  ethyl 
acetate.  (Hamers,  Dissert.  1906);  (Naumann 
B.  1910,  43.  314.) 

1.49  g.  AgBr  is  dissolved  in  1  1.  of  1%  thio- 
carbamide+Aq.  (Mees  and  Piper,  Photog. 
J.  1912,  36.  239.) 

Insol.  in  warm  pyridine. 

Mol.  wt.  determined  in  piperidine.  (Wer- 
ner, Z.  anorg.  1897,  15.  16.) 

Min.  Bromyrite,  Bromite. 

Silver  bromide  ammonia,  AgBr,  NH3. 

(Joannis  and  Crozier,  C.  R.  894, 118.  1150.) 


AgBr,  1^NH3.  (Jarry,  A.  ch.  1899,  (7) 
17.  356.) 

2 AgBr,  3NH3,     (Joannis  and  Crozier.) 

AgBr,  3NH3.  Decomp.  by  H2O.  SI.  sol.  in 
liquid  NH3.  (Jarry.) 

AgBr,  5NH3.  (Jarry,  C,  R.  1898,  126. 
1141.) 

Silver  carbide,  Ag4C. 

(Gay-Lussac.)  . 

Ag2C(?).  Sol.  in  HNOg+Aq  with  residue 
ofC.  (Liebig,  A.  38.  129.) 

Ag2C2.  Sol.  in  HNO3+Aq  with  residue  of 
C.  (Regnault,  A.  19.  153.) 

Silver  swfrchloride,  Ag4Cl3. 

NH4OH+Aq  dissolves  the  greater  part, 
the  residue  (20%)  being  sol.  in  HNO3+Aq. 
KCN  dissolves  the  greater  part;  H2SO4  dis- 
solves about  2%;  acetic  acid  and  KOH  are 
without  action.  (Bibra,  J.  pr.  1875,  (2)  12. 
52.) 

Argentous  chloride,  Ag2Cl. 

Obtained  in  a  pure  state  by  Guntz  (C.  R. 
112.  861).  Dil.  HNO3+Aq  does  not  attack 
but  warm  cone.  HNO3+Aq  decomp.  Easily 
sol.  in  KCN+Aq.  (Guntz,  C.  R.  112.  1212.) 

The  following  data  are  for  a  more  or  less 
impure  Ag2Cl. 

Boiling  cone.  HCl+Aq,  NaCl+Aq,  or  NH4OH+Aq 
dissolve  out  AgCl,  and  leave  Ag.  (Scheele,  Wetzlar, 
Bulk,  Wohler.) 

According  to  Berthollet,  wholly  sol.  in  NH4OH  +Aq. 

Sol.  for  the  most  part  in  NH^OH-f-Aq,  and  the  resi- 
due is  sol.  in  HNOs+Aq  (  =Ag  +AgCl).  (v.  Bibra,  B. 
7.  741.)  . 

Silver  chloride,  AgCl. 

Nearly  insol.  in  H2O. 

When  AgCl  is  left  in  contact  for  some  hours 
with  pure  H2O  at  20-22°,  and  especially  at  75°, 
traces  go  into  solution;  more  Cl  is  dissolved 
than  Ag.  When  1  pt.  Ag  is  pptd.  as  AgCl  in 
presence  of  1  million  pts.  H2O  a  slight  bluish 
milkiness  is  observed;  but  in  order  to  have  a 
distinct  ppt.  4  pts.  Ag  should  be  present. 

Dil.  HNO3+Aq  does  not  increase  the  solu- 
bility of  AgCl,  but  AgCl  is  not  absolutely 
insol.  in  stronger  HNO3+Aq.  (Mulder.) 

I  pt.  AgNO3,  when  mixed  with  HCl+Aq 
in  presence  of  120.000  (Pfaff),  240,000  (Hart- 
ing),  pts.  H2O,  causes  an  opalescence. 

1  pt.  Ag  gives  a  slight  turbidity  with  HC1  + 
Aq  in  presence  of  200,000  pts.  H2O,  a  scarcely 
opalescent  cloudiness  with  400,000  pts.  H2O, 
and  the  same  after  the  lapse  of  15  minutes 
in  presence  of  800,000  pts.  H2O.  (Lassaigne.) 

I  pt.  Ag  can  be  detected  as  AgCl  in  1  mil- 
lion parts  H2O  at  ordinary  temp.,  but  not 
in  2  million  parts.  In  NaNO3+Aq  containing 
0.79  pt.  NaNO3  in  200,000  pts.  H2O,  1  pt.  Ag 
can  be  detected  as  AgCl.  This  dissolves  at 
75°,  and  is  visible  again  on  cooling. 

If  the  same  liquid  contains  1574  pts.  NaNOj, 
the  AgCl  remains  in  solution  after  cooling. 


822 


SILVER  CHLORIDE 


In  100  ccm.  H2O  containing  0.787  g.  NaNO3, 
13  drops  of  NaCl  and  silver  solution,  each 
drop  of  which  contains  0.05  mg.  Ag,  cause  a 
precipitate  at  5°,  20  drops  at  15-17°,  60  drops 
at  45-55°. 

AgCl  is  somewhat  less  sol.  in  HNO3+Aq 
than  in  NaNO3+Aq  when  the  amount  of  H2O 
remains  the  same. 

Therefore,  if  HC1  is  used  instead  of  NaCl, 
about  lli  less  AgCl  remains  in  solution. 

In  100,000  pts.  of  H2O,  which  contain  HNO3 
and  an  amount  of  HCl  corresponding  to  the 
amount  of  Ag  salt,  1.596  pts.  AgCl  dissolve 
at  25°.  The  solution  is  precipitated  by  either 
AgNO3  or  HC1.  (Mulder,  Silber  "Probir- 
methode,  Leipzig,  1869.  62.) 

(For  further  older  data,  see  Storer's  Dic- 
tionary.) 

White  flaky  AgCl  is  appreciably  sol.  in  hot 
H2O,  1000  ccm.  boiling  H2O  dissolving  about 
2  mg.  AgCl.  Far  less  sol.  in  H2O  containing 
AgNO3,  being  practically  insol.  in  H2O  con- 
taining 0.1  g.- AgNO3  in  a  litre.  Solubility  is 
also  diminished  one-half  by  addition  of  HC1. 
(Cooke,  Sill.  Am.  J.  (3)  21.  220.) 

Solubility  in  H2O  rapidly  diminishes  as  the 
temp,  falls.  (Cooke,  I.  c.) 

Not  completely  insol.  in  H2O.  According 
to  Stas  (C.  R.  73.  998)  there  are  four  modifica- 
tions: (1)  gelatinous;  (2)  cheesy-flocculent; 
(3)  pulverulent;  (4)  granular,  crystalline,  or 
fused.  (4)  is  almost  absolutely  insol.  in  H2O  at 
the  ordinary  temp.,  but  the  solubility  in- 
creases with  the  temp.,  and  is  considerable 
at  100°;  (2),  which  is  formed  by  the  pre- 
cipitation of  a  cold  dilute  Ag  solution,  has 
the  greatest  solubility  in  pure  H2O;  and  it 
changes  its  solubility  by  standing,  or  if  made 
pulverulent  by  shaking  with  H2O;  (3)  is  also 
sol.  in  H2O;  the  solution  of  (2)  or  (3)  in  pure 
H2O,  or  H2O  acidified  with  HNO3,  is  precipi- 
tated by  AgNO3  or  NaCl+Aq. 

In  order  to  ppt.  1  pt.  AgCl  in  above  solu- 
tion 3  pts.  of  Cl  as  chloride  or  Ag  as  nitrate 
are  necessary;  the  pptn.  is  then  complete. 

Solubility  of  granular  variety  in  boiling 
H2O  is  proportionately  large,  and  pptn.  is 
brought  about  by  3  pts.  Cl  or  Ag  as  above, 
but  the  pptn.  in  this  case  is  not  complete. 

The  salts  formed  simultaneously  with  the 
AgCl  have  no  influence  on  the  solubility  of  the 
AgCl.  Presence  of  HNO3  does  not  increase 
the  solubility  of  (2),  but  has  that  effect  on 
(3)  in  proportion  to  the  amt.  of  HNO3  pre- 
sent. (Stas,  C.  R.  73.  998.) 

Further  determination  by  Stas  are  as 
follows: — 

Between  0°  and  30°  granular  AgCl  is  insol. 
in  pure  H2O,  or  H2O  acidulated  with  HNO3. 

Between  0°  and  30°  the  flocculent  and  pul- 
verulent forms  of  AgCl  dissolve  without 
alteration  in  pure  H2U,  in  acidulated  H2O, 
in  alkali  acetates +Aq,  and  in  Hg(C2H3O2)2 
+Aq  containing  an  alkali  acetate.  Their 
degree  of  solubility  is  a  function  of  the  state 
of  the  chloride,  of  the  temp.,  and  of  the  nature 


and  quantity  of  the  solvent  within  these 
limits  of  temp.  (0°-30°).  These  solvents,  if 
they  contain  either  Ag  in  the  state  of  an  Ag 
salt,  or  Cl  as  chloride  or  HCl  in  an  amount 
three  times  that  which  they  can  dissolve  as 
AgCl,  exercise  no  solvent  action  on  any  of  the 
modifications  of  AgCl.  And  reciprocally  sat. 
AgCl+Aq  is  pptd.  instantly  by  a  decinormal 
solution  of  AgNO3  or  MCI. (or  HCl).  The 
AgCl  is  wholly  pptd.  when  the  quantity  of 
the  Ag  or  Cl  thus  added  is  equal  to  three 
times  the  quantity  of  the  Ag  or  Cl  dissolved 
as  AgCl. 

Between  50°  and  100°,  however,  decinormal 
solutions  of  Ag  or  chlorides,  which  cause 
instant  ppts.  in  solutions  sat.  with  any  of  the 
modifications  of  AgCl,  do  not  eliminate  all 
the  dissolved  AgCl.  At  100°,  they  only  ppt. 
60%  of  the  amt.  dissolved.  (Stas,  A.  ch.  (5) 
3.  323.) 

Calculated  from  electrical  conductivity  of 
AgCl  +Aq,  AgCl  is  sol.  in  715,800  pts.  H2O 
at  13.8°,  and  384,100  pts.  at  26.5°.  (Holle- 
man,  Z.  phys.  Ch.  12.  132.) 

Calculated  in  the  same  way,  1.  1.  H2O 
dissolves  0.76  mg.  at  2°;  0.97  mg.  at  10°;  1.52 
mg.  at  18°;  2.24  mg.  at  26°;  3.03  mg.  at  34°; 
4.05  mg.  at  42°.  (Kohlrausch  and  Rose,  Z. 
phys.  Ch.  12.  242.) 

Solubility  in  H2O  =  1.25X10-5mol./l.  at  25°. 
(Goodwin,  Z.  phys.  Ch.  1894,  13.  645.) 

Solubility  of  AgCl  in  H2O  at  25°  is  1.41X 
10-5  fin  normality).  (Thiel,  Z.  anorg.  1900, 
24.  57.) 

2.16  X 10 -5  moles  are  sol.  in  1  liter  H2O  at 
25°.  (Noyes  and  Kohr,  Z.  phys.  Ch.  1903, 
42.  341.) 

1.53X10~3  g.  per  liter  are  dissolved  in  sat. 
aq.  solution  at  20°.  (Bottger,  Z.  phys.  Ch. 
1903,  46.  603.) 

1  1.  H2O  dissolves  1.6  mg.  AgCl  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1904,  50.  356.) 

21.8  milligrams  are  dissolved  in  1  liter  of 
sat.  solution  at  100°.  (Eottger,  Z.  phys.  Ch. 
1906,  66.  93.) 

1.34  mg.  are  contained  in  1  1.  of  sat.  solu- 
tion at  18°.  (Kohlrausch,  Z.  phys.  Ch.  1908, 
64.  168.) 

1 1.  sat.  solution  at  t°  contains  mg.  AgCl. 


t 

mg.  AgCl 

t 

mg.  AgCl 

1.55 
4.68 
9.97 

0.56 
0.66 
0.89 

17.51 
25.86  . 
34.12 

.  1.31 
1.935 
2.74 

(Kohlrausch,  Z.  phys.  Ch.  1908,  64.  168.) 

Solubility  in  H2O  =  1.6X10-5  g.-mol.  per 
litre  at  25°.  (A.  E.  Hill,  J.  Am.  Chem.  Soc. 
1908,  30.  74.) 

1  1.  H2O  dissolves  0.00154  g.  AgCl  at  21°; 
0.0217  g.  at  100°.  (Whitby,  Z.  anorg.  1910, 
67.  108.) 


SILVER  CHLORIDE 


823 


Calculated  from  electrical  conductivity  o: 
AgCl-f-Aq,  l  1.  H2O  dissolves: 

0.0105  milli-equivalents  AgCl  at  18°. 

0.0365      "  "  "     "  50°. 

0.147        "  "      "  100°. 

(Melcher,  J.  Am.  Chem.  Soc.  1910,  32.  55.; 

1  1.  H2O  dissolves  1.02X10-5  g.  equiv.  at 
18°;  1.429  X  10~5  g.  equiv.  at  25°.  (van  Rossen 
C.  C.  1912,  I.  1539.) 

The  most  probable  average  value  for  solu- 
bility of  AgCl  in  H2O  is  1.04XH)-5  g.  equiv 
per  1.  at  18°,  and  1.43X10-5  g.  equiv.  per  1 
at  25°.  (van  Rossen,  C.  C.  1912,  II.  1807.) 

1.20X10-6  g.  AgCl  are  sol.  in  1  1.  H2O  at 
18°.  (Glowczynski,  C.  A.  1916,  741.) 

More  sol.  in  H2O  than  AgSCN.  (Normand, 
Chem.  Soc.  1912,  101.  1853.) 

Sol.  in  cone.  HCl+Aq,  and  also  when  not 
very  cone.;  thus  the  solution  of  1  pt.  AgNO3  + 
Aq  in  15,000  pts.  H2O  is  clouded  by  a  little 
HCl+Aq,  but  clears  up  by  the  addition  of 
more.  (Reinsch,  J.  pr.  13.  133.) 

1  pt.  AgCl  dissolves  in  200  pts.  cone.  HC1+ 
Aq  and  in  600  pts.  HCl+Aq  diluted  with 
pts.  H2O.     (Pierre,  J.  Pharm.  (3)  1?.  237.) 

Somewhat  sol.  in  hot  alcohol,  to  which  HCJ 
has  been  added,  but  is  precipitated  on  cooling 
(Erdmann,  J.  pr.  19.  341.) 

100  pts.  sat.  HCl+Aq  (sp.  gr.  1.165)  dis- 
solve 0.2980  pt.  AgCl,  or  AgCl  is  sol.  in  336 
pts.  HCl+Aq  at  ord.  temp.;  100  pts.  HC1  + 
Aq  Csp.  gr.  1.165)  at  b.-pt.  dissolve  0.56  g. 
AgCl,  or  AgCl  is  sol.  in  178  pts.  HCl+Aq. 

Solubility  of  AgCl  in  dil.  HCl+Aq.  100 
ccm.  HCl+Aq  (sp.  gr.  1.165),  to  which  the 
given  amt.  H2O  has  been  added,  dissolve  g. 
AgCl. 


ccm. 
HCl 

ccm. 
H20 

Agfcl 

Pts.  HCl 

which  dis- 
solve 1  pt. 
AgCl 

100 
100 

100 
100 

10 
20 

30 

50 

0.056 
0.018 
0.0089 
0.0035 

1,785 
5,555 
11,235 
18,571 

(Vogel,  N.  Rep.  Pharm.  23.  335.) 

If  HCl  is  added  to  a  solution  in  which 
Vi.ooo.ooo  pt.  Ag  is  suspended,  the  milkiness  dis- 
appears. Solubility  in  HCl+Aq  increases 
with  the  temp.,  the  AgCl  separating  out  on 
cooling.  (Mulder.) 

The  amounts  of  AgCl  which  dissolve  in 
HCl+Aq  are  directly  proportional  to  the 
volumes  of  acid  (of  fixed  concentration)  used. 
(Barlow,  J.  Am.  Chem.  Soc.  1906,  28.  1448.) 

11.    1  %  HCl  dissolves  0.0002  g.  AgCl  at  21°. 

1 1.    5%  HCl  dissolves  0.0033  g.  AgCl  at  21°. 

1 1.  10%  HCl  dissolves  0.0555  g.  AgCl  at  21°. 

(Whitby,  Z.  anorg.  1910,  67.  108.) 


Solubility  in  HCl+Aq  at  25°. 


HCl 

g.-equivalents  per  1. 


0.649 
1.300 
1.911 
2.149 
2.569 
2.975 
3.576 
4.182 
4.735 
5.508 


Ag  x  10-3 

g.-equivalents  per  1. 


0.032 
0.126 
0.266 
0.374 
0.610 
0.814 
1.358 
2.147 
3.168 
4.126 


(Forbes,  J.  Am.  Chem.  Soc.  1911,  33.  1941.) 


Solubility  in  20%  HCl  +Aq. 


HCl 

N/10 
AgN03 
ccm. 

Opalescent 
at  t° 

G.  AgCl  to 
100  g.  anhy- 
drous HCl 

20  g.  of 

1.0 

20%  acid 

1.1 

0.0 

0.39 

2.0 

29.5 

0.72 

3.0 

51.5 

1.076 

3.75 

70.0 

1.346 

4.25 

82.0 

1.525 

4.75 

90.0 

1.74 

5.80 

107.0 

2.08 

(Lowry,  Roy,  Soc.  Proc.  1914,  91.  A.  62.) 


SI.  sol.  in  cone.  HBr+Aq.    (Lowig.) 
Insol.     in     HNO3+Aq.       (Wackenroder.) 
Entirely  unacted  upon  by  HNO3  of  1.43 
sp.  gr.    (Wurtz,  Am.  J.  Sci.  (2)  25.  382.) 

Solubility  in  dil.  HNO3+Aq  is  the  same  as 
solubility  in  H2O,  i.  e.  l/ 2,000,000  pt.  of  Ag  can- 
not be  detected  in  H2O  with  or  without  HNO3, 
but  Vi.ooo.ooo  pt.  can  be  detected  in  both  cases. 
(Mulder.) 

1  pt.  Ag  in  the  form  of  AgCl  dissolves  at 
25°  in  83,000  pts.  H2O  containing  free  HNO3 
and  0.33  pt.  of  HCl.  (Mulder.) 

100,000  pts.  cone.  HNO3+Aq  dissolve 
about  2  pts.  AgCl,  and  solubility  is  not  sen- 
sibly affected  by  lower  nitrogen  oxides. 
(Thorpe,  Chem.  Soc.  (2)  10.  453.) 


Solubility  of  AgCl  in  HNO3+Aq  at  25°. 


G.  per  liter 

HNOs 

AgCl 

HNOs 

AgCl 

0.0315 
0.063 
0.630 

0.001647 
0.001705 
0.00176 

18.9 
94.5 

0.00225 
0.0245 

(Glowczynski,   Kolloidchem.  Beih.   1914.   6. 

147.) 

824 


SILVER  CHLORIDE 


Insol.  in  cold  cone. 

H2SO4,  but 

on  boiling 

Solubility  in  NH4OH+Aq  at 

25°. 

is  in  part  decomp.  and 

in  part  dissolved,  and 

does  not  separate  on  cooling. 

g.  at.  Ag        Mols.  NHs 

g.  at.  Ag 

Mols.  NH3 

AgCl  is  not  more  sol.  in  dil.  H2SO4+Aq 

per   .                 per  1. 

perl. 

per  1. 

.1       •     j*i 

crxrn    i   A  ^ 

man  in  011.  j.j..i.>ivy3-p-ri-»-i' 
Unacted  upon  by  cold  H2SO3+Aq,  and  but 

0.151           2.042 

0.0140 

0.253 

slightly  decomp.  on  heating.    (Vogel.) 

0.149           2.017 

0.0140 

0.253 

Abundantly  sol.  in 

H2PtCl4+Aq  without 

0.149           2.013 

0.0140 

0.252 

decomp.    (Birnbaum,  Z.  Ch.  1867. 

520.) 

0.147           1.991 

0.0139 

0.252 

Insol.  in  cold  dil.  caustic  alkalies  +Aq  but 

0.0616         0.961 

0.00621 

0.118 

decomp.  by 

hot  cone. 

solutions.    (Gregorv.) 

0.0583         0.916 

0.00621 

0.118 

Decomp. 

by  K2C03 

+Aq. 

0.0584         0.909 

0.00619 

0.118 

SI.  sol.  in 

cold  K2CO3+A"q. 

0.0572         0.903 

0.00625 

0.118 

Easily  sol 

.  even  in  dil.  NH4OH+Aq. 

0.0569         0.896 

0.00304 

0.0590 

1  pt.  AgCl  dissolves 

in  1288  pts. 

NH4OH  + 

0.0555         0.873 

0.00297 

0.0589 

Aq  of  0.89 

sp.  gr.     (Wallace  and  Lamont, 

0.0541         0.863 

0.00300 

0.0585 

Chem.  Gaz. 

1893.  137 

) 

0.0514         0.818 

0.05149 

0.0288 

100  pts.  NH4OH+Aq  of  0.986  sp.  gr.  dis- 

0.0249        0.428 

0.00143 

0.0287 

solve  at  80°  1.492  pts 

AgCl,  drie 

d  at  100°. 

0.0240         0.416 

0.00142 

0.0285 

(Pohl,  W.  A 

.  B.  41.  627.) 

0.0235         0.411 

0.00141 

0.0282 

1  1.  NH4C 

VFr_l_A«  nt 

O  QAQ  er>     o-r 

rHaanlvAQ 

0.0227         0.397 

51.6  g.  Ag  as  freshly  precipitated  AgCl,  and 

47.6  g.  when  diluted  with  1  1.  H2O. 
1  1.  NH4OH+Aq  of  0.924  sp.  gr.  dissolves 
58  g.  Ag  as  freshly  precipitated  AgCl;  1  1. 
NH4OH+Aq  of  0.899  sp.  gr.  dissolves  49.6 

(Whitney  and  Melcher,  J.  Am.  Chem.  Soc. 
1903,  26.  78.) 

g.;  0.5  1.  NH4OH+Aq  (of  0.049 

sp.  gr.)  + 

0.5  1.  saturated  NaCl+Aq  dissolves  20.8  g.; 
0.5  1.  NH4OH+Aq  (of  0.949  sp.  gr.)+0.  5  1. 

Solubility  of  AgCl  in  NH4OH+Aq  at  25°. 

saturated  KCl+Aq  dissolves  20.4 

g.;  0.5  1. 

Ag  =  g.  at.  Ag  in  1000  g.  H2O. 

NH4OH+Aq  (of  0.949  sp.  gr.)+0.5  1.  satu- 

NH3 =  g.  mol.  NH3  in  1000  g.  H2O. 

rated  NH4Cl+Aq  dissolves  22.4  g.     Ag  as 

Cone.  =  Molecular    concentration    of    free 

freshly  pptd.  AgCl.  (Millon  and  Commaille, 

NH3. 

C.  R.'  66.  309.) 

1    g.    AgCl    dissolves    in    428.64    g.    5% 

Ag 

NH3 

Cone. 

Solid  phase 

NH,iOH4-A 

rt   (an     nrr     f 

QQS^  of  19° 

•  1  g.  AgCl 

JA  A-L4\JH    l^-**-M   V'-M"'*    &*  •    v>vt-'v-'/    *-*v    -••*• 

dissolves  in  12.76  g.  10%  NH4OH  + 

Aq(sp.  gr. 

0.023 

0.437 

0.391 

AgCl 

0.96)  at  18°.     (Longi, 

Gazz.  ch.  it.  13.  87.) 

0.025 

0.428 

0.378 

f 

1  g.  freshly  pptd.  AgCl  is  sol.  in  17  ccm. 
10%  NH4OH+Aq.    Solubility  is  diminished 

0.1197 
0.1308 

1.700 

1.688 

1.461 
1.426 

< 

by  presence  of  AgBr 

(Senier, 

Pharm.   J. 

0.372 

3.782 

3.038 

« 

Trans.  (3)  14.  1.) 

0.378 

3.945 

3.181 

1 

0.574 

5.10 

3.95 

' 

0.609 

5.33 

4.11 

' 

Solubility  in  NH4OH+Aq  at  0°. 

0.633 
0.745 

5.545 
6.26 

4.279 

4.77] 

AgCl+2AgCl,  3NH3 

G.  per  100 

g.  solution. 

0.754 

6.27 

4.76  1 

' 

0.757 

6.25 

4.74  f 

1 

NH3 

AgCl 

NHs 

AgCl 

0.760 
0.775 

6.25 
6.52 

4.73  1 
4.97 

2AgCl, 

3NH3 

1.45 

0.49 

28.16 

5.69 

0.848 

8.28 

6.58 

1.94 

1.36 

29.80 

7.09 

0.968 

11.19 

9.25 

' 

5.60 

3.44 

30.19 

7.25 

0.980 

11.78 

9.82 

' 

6.24 

4.00 

32.43 

5.87 

0.978 

12.23 

10.27 

11.77 

4.68 

34.56 

4.77 

0.965 

12.26 

10.33 

' 

16.36 

5.18 

37.48 

3.90 

1.03 

12.68 

10.62 

' 

1.09 

12.96 

10.78 

' 

1  049 

14.34 

12.24 

( 

(Jarry,  A.  ch.  1899,  (7)  17.  342.) 

1^039 

14.47 

12.39 

' 

Solubility  in  NH4OH-f-Aq  increases  with 
the  temp.     (Jarry.) 


(Straub,  Z.  phys.  Ch.  1911,  77.  332.) 


Easily  (Brett),  difficultly  (Wittstein),  sol 
in  NH4Cl+Aq,  but  not  in  other  NH4  salts. 


SILVER  CHLORIDE 


825 


Solubility  in  NH4Cl+Aq  at  15°. 


NH4C1 


10.0 

14.29 

17.70 

19.23 

21.98 

25.31 

28.45 

Sat. 


%  AgCl 


0.0050 

0.0143 

0.0354 

0.0577 

0.110 

0.228 

0.340* 

0.177 


*24.5°. 
(Schierholz,  W.  A.  B.,  1890,  101.  2b.  8.) 

Solubility  in  NH4Cl+Aq  (26.31%)  at  t° 

%  AgCl 


15 

40 

60 

80 

90 

100 

110 


0.276 
0.329 
0.421 
0.592 
0.711 
0.856 
1.053 


(Schierholz.) 

At  25°,  1  1.  NH4Cl+Aq  containing  0.00053 
g.  NH4C1  dissolves  0.001604  g.  AgCl;  0.00530 
g.  NH4C1,  0.002379  g.  AgCl.  (Glowczynski, 
Kolloidchem.  Bern.  1914,  6.  147.) 

See  also  Forbes,  page  826. 

1  1.  KClO3+Aq  dissolves  1.8  mg.  (Guye, 
J.  Chim.  Phys.  10.  145.) 

SI.  sol.  in  cone.  KCl+Aq,  NaCl+Aq,  and 
certain  other  chlorides. 

NaCl,  KC1,  NH4C1,  CaCl2,  ZnCl2+Aq,  etc., 
dissolve  appreciable  quantities  of  AgCl,  es- 
pecially if  hot  and  concentrated,  but  it  sep- 
arates out  for  the  most  part  on  cooling, 

Sol.  in  solutions  of  all  the  metallic  chlorides 
which  are  sol.  in  H2O,  thus  NaCl,  KC1,  CaCl2, 
SrCl2,  and  BaCl2+Aq  all  dissolve  AgCl,  espe- 
cially if  hot.  MgCl2,  NH4C1,  and  HgCl2 
(least)  also  dissolve  AgCl.  (Mulder.) 

Sol.  in  cone.  CaCl2+Aq.    (Wetzlar.) 

Sol.  in  roseocobaltic  chloride +Aq.  (Gibbs 
and  Genth.) 

Insol.  in  SnCl4,  HgCl2,  CuCl2,  ZnCl2,  CdCl 
NiCl2,  or  CoCl2+Aq.    (Vogel.) 

Solubility  of  AgCl  in  sat.  solutions  of  chlorides 


Experiments  by  Hahn  give  different  results 
Tom  those  of  Vogel  as  follows:  — 

Solubility  in  various  salts  +Aq. 

Salt 

%  salt 

Sat. 

at  t° 

%  AgCl 

KC1. 
NaCl           .      . 
NH4C1  .      .      . 

CaCl2     .      .      . 
MgCl2          .      . 
BaCl2     .      .      . 
FeCl2     .      .      . 
FeCl3      .      .      . 
MnCl2    .      .      . 
ZnCl2     .      .      . 
CuCl2     .      .      . 
PbCl2     .      .      . 

24.95 
25.96 
28.45 
41.26 
36.35 
27.32 

19.6 

« 

24.5 

« 
."   . 

24  '.5 

24^5 

t( 

0.0776 
0.1053 
0.3397 
0.5713 
0.5313 
0.0570 
0.1686 
0.0058 
0.1996 
0.0134 
0.0532 
0.0000 

(Hahn,  Wyandotte    Silver  Smelting  Works, 
1877.) 

1  1.  4-N  KCl+Aq  dissolves  0.915  g.  KC1  at 
25°.    (Hellwig,  Z.  anorg.  1900,  25.  166.) 

Solubility  in  KCl+Aq  at  t°. 

t° 

G.  equiv.  per  1. 

AgXlO-a 

KC1 

1.0 
25.0 
35.0 

1.734 
2.415 

2.786 

3.325 
3.083 
2.955 

(Forbes,  J.  Am.  Chem.  Soc.  1911,  33.  1937.) 

Solubility  in  KCl+Aq  at  25°. 
G.  per  liter. 


KCl 

AgCl 

KCl 

AgCl 

0.00236 
0.00471 

0.00184 
0.00218 

0.01491 
0.02984 

0.00305 
0.00321 

(Glowczynski,   Kolloidchem.   Beih.   1914,   6. 
147.) 

Solubility  in*CaQ2+Aq. 


at  ordinary  temperatures. 

Salt 

100  pts.  sat. 
solution  dissolve 
pts.  AgCl 

Pts.  solution 
required  to  dis- 
solve 1  pt. 
AgCl 

BaCl2 

0.0143 

6,993 

SrCl2      .      .      . 

0.0884 

1,185 

CaCl2     .      .      . 

0.0930 

1,075 

NaCl      .      .      . 

0.0950 

1,050 

KCl       ... 

0.0475 

2,122 

NH4C1   .      .      . 

0.1575 

634 

MgCl2         .     . 

0.1710 

584 

HC1        ... 

0.2980 

336 

(Vogel,  N.  Rep.  Pharm.  23.  335.) 

t 

G.  equiv.  per  1. 

AgXlO" 

CaCP 

2 

1.0 
25.0 
35.0 

0.964 
1.514 
1.806 

3.512 
3.320 
3.221 

(Forbes,  1.  c.) 

Sat.  CuCl2+Aq  at  0°  dissolves  2.835  g. 
AgCl  per  1;  at  100°,  8.147  g.  Solubility  in 
sat.  MgCl2+Aq  is  still  greater.  (Hahn,  Eng. 
Min.  J.  65.  434.) 


826 


SILVER  CHLORIDE 


More   sol.    in    HgCl2+Aq    than   in    H2O. 

Solubility  in  salts  +Aq  at  25°. 

(Finzi,  Gazz.  ch.  it.  1902,  32.  (2)  324.) 
At  15°,  100  g.  NaCl  in  280  ccm.  H2O  dis- 
solve 485  mg.  AgCl;  100  g.  KC1  in  300  ccm. 

C  =  concentration  of  the  salt  in  salt  solution 
in  g.-equivalents  per  litre. 

H2O  dissolve  334  mg  •  100  g   NH4C1  in  280 

ccm.  H2O  dissolve  1051  mg. 

Salt 

c 

AgX  10-3 

The    solubility    decreases    with    dilution 

g.-equivalents  per  1. 

rapidly  at  first  until  about  an  equal  vol.  of 
H2O  has  been  added,  and  then  much  more 
slowly  to  a  minimum  quantity,   when  the 
dilution  is  1  :  10  for  NaCl  and  KC1,  and  1  :  20 
for  NH4C1. 
100  g.  NaCl  in  280  ccm.  H2O  dissolve  2170 
mg.  AgCl  at  109°;  100  g.  NH4C1  in  280  ccm. 
H2O  dissolve  4000  mg.  AgCl  at  110°;  100  g. 
NaCl  in  620  ccm.  H2O  (14%  solution)  dissolve 
15  mg.  AgCl  at  15°,  and  774  mg.  at  104°. 
(Schierholz,  W.  A.  B.  101,  2b.  4.) 
The  solubility  of  AgjCl  in  NaCl+Aq  de- 
creases   with    diminishing    concentration    of 
NaCl+Aq.      (Barlow,   J.   Am.   Chem.   Soc. 

NaCl 

0.933 
1.190 
1.433 
1.617 
1.871 
2.094 
2.272 
2.449 
2.658 
2.841 
3.000 
3.270 
3.471 
3  747 

0.086 
0.130 
0.184 
0.245 
0.348 
0.446 
0.570 
0.684 
0.851 
1.040 
1.194 
1.583 
1.897 
4  462 

1906,  28.  1448.) 

3.977 

2.879 

4.170 

3.335 

.  Solubility  in  NaCl+Aq. 

4.363 
4.535 

3.810 

4.298 

Gravimetric  measurements,  15° 

5.039 

6.039 

Strength  of  salt  solution 

G.  AgCl  retained  per 
100  g.  NaCl 

CaCl2 

1.748 
2.201 

0.289 
0.501 

2 

15%  NaCl 
20%  NaCl 
28%  NaCl 

0.063 
0.134 
0.279 

2.741 
3.264 
3.737 
4.033 

0.900 
1.463 

2.182 
2.802 

4.538 

4.175 

Volumetric  measurements 

5.005 

5.823 

NaCl 

N/10 
AgNO3 
ccm. 

Opal- 
escent 
att° 

G.  AgC 
retained 
per  100  g. 

•vrn/-ii 

NH4C1 

0.513 
0.926 

0.042 
0.113 

1.141 

0.172 

20  g.  of  15%  solution 

0.25 
0.4 

28 

40 

0.119 
0.191 

1.574 
2.143 

0.365 
0.842 

0.7 

64 

0.335 

2.566 

1.425 

1.0 
1.25 
1.7 

78 
89 
102.5 

0.478 
0.598 
0.812 

2.918 
3.162 
3.510 

2.  160 
2.795 
4.029 

4.  -363 

9.353 

20  g.  of  20%  solution 

0.43 
0.65 

17.0 
26.0 

0.156 
0.234 

4.902 
5.503 

14.92 
24.04 

0.82 

37.0 

0.295 

5.764 

30.17 

1.2 
1.6 
2.12 
2.52 

51.5 
67.0 
79.5 

88.5 

0.430 
0.524 
0.765 
0.910 

SrCl2 

0.550 
0.989 
1.359 

0.033 
0.092 
0.173 

2 

3.08 

97.0 

1.10 

1.572 

0.236 

v3.52 

105.0 

1.27 

1  .698 
1.818 

0.284 
0.348 

20  g.  of  28%  solution 

2.25 
2.75 
3.5 
4.5 

36.5 
45.0 
56.0 
69.0 

0.675 
0.704 
0.896 
1.153 

2.140 
2.476 
2.992 
3.494 

0.510 
0.747 
1.252 
2.018 

5.5 

84.0 

1.411 

4.  152 

3  .  594 

6.5 
7.75 

94.0 
107.5 

1.664 
1.958 

5.216 
5.775 

8.  174 
12.04 

(Lowry,  Roy,  Soc.  Proc.  1914,  91.  A,  61.) 

SILVER  CHLORIDE 


827 


Solubility  in  salts  +Aq.  at  25°  —  Continued. 

presence  of  NaC2H3O2  or  NH4OH+Ao.  AgCl 
is  pptd.  from  above  solution  by  NaC2H3O2  + 
Aq.    (Mulder.) 
Sol.  in  Hg(NO3)2+Aq  (Wackenroder,  A. 
41.  317);  in  considerable  amount  (Liebig,  A. 
81.  128);  and  is  precipitated  by  HC1,  NH4C1, 
NaCl,  KC2H3O2  (Debray,  C.  R.  70.  849);  in- 
completely precipitated  by  AgNO3  and  not  by 
HNO3  (Wackenroder). 

Solubility  of  AgCl  in  Hg(NO3)2+Aq  at  25°. 
(G.  mols.  per  1.) 

Salt 

C 

AgXlO-3 
g.-equivalents  per  1. 

KC1 

1.111 
1.425 
1.713 
2.022 
2.396 
2.628 
2.850 
3.081 
3.424 
3.843 

0.141 
0.235 
0.391 
0.616 
1.050 
1.390 
1.845 
2.435 
3.602 
5.725 

BaCl2 

1.248 
1.610 
2.676 
3.260 

0.186 
0.339 
1.274 
2.366 

Hg(N03)2 
HNOs 

AgCl 

Hg(N03)2 
HNOs 

AgCl 

2 

0.0100 
0.0125 
0.025 

0.00432 
0.00499 
0.00690 

0.050 
0.100 
1.000 

0.00914 
0.01395 
0.04810 

(Forbes.  J.  Am.  Chem.  Soc.  1911.  33.  1940). 

Sol.  in  NaNO3,  KNO3,Ca(NO3)2,Mg(NO3)2, 
and  NH4NO3-}-Aq;  si.  sol.  at  ord.  temp.,  but 
solubility  is  much  increased  by  heat. 

Solubility  in  NaNO3+Aq  at  15-20°. 


ccm.  H2O 

1 

g- 

NaNOs 

mg.  AgCl 
dissolved 

100 
200 
300 
100 

to  to  o  o 

787 
787 
361 
787 

1 
1 

3 
2 

33 
.93 
99 
53 

Solubility  increases 

with 

ascending 

temp 

. 

Temp. 

ccm.  H2O 

g 

.  NaNOs 

mg.  AgCl 
dissolved 

5° 
15-17° 
18° 
30° 
45-55° 

100 
100 
100 

100 
100 

O  OO  O  O 

.787 
.787 
.787 

.787 
.787 

0.86 
1.33 
1.46 
2.33 
3.99 

(Mulder.) 

At  25°,  100,000  pts.  H2O  containing  a  little 
free  HNO3  and  0.787  g.  NaNO3  dissolve  2.128 
mg.  AgCl.  By  adding  2  g.  more  NaNO3  to 
above  solution,  2.5269  mg.  (Vs  more)  AgCl  are 
dissolved.  (Mulder.) 

Solubility  in  H2O  is  not  appreciably  in- 
fluenced by  Vio  N  to  N-KNO3  or  NH4NO3- 
Aq.    (van  Rossen,  C.  C.  1912,  II.  1807.) 

In  presence  of  NaNO3  and  excess  of  HC1, 
1  1.  H2O  dissolves  0.03  mg.  AgCl.  (Richards 
and  Wells.) 

Hg(NO3)2+Aq  dissolves  considerable  quan- 
tities of  AgCl,  but  the  other  nitrates  do  not 
(Mulder.) 

Much  more  sol.  in  hot  than  in  cold 
Hg(NO3)2+Aq,  and  much  more  sol.  therein 
than  in  NH4NO3+Aq.  NaCl  ppts.  AgCl 
from  this  solution;  much  less  sol.  therein  in 


HNO3  was  present  in  all  cases,  and  it  was 
found  that  there  was  no  difference  in  solubil- 
ity of  AgCl  with  concentrations  between  0.1N 
and  2N  HNO3.  (Morse,  Z.  phys.  Ch.  1902, 
46.  708.) 

Not  sol.  to  appreciable  extent  in  Cu(NO3)2, 
Fe2(NO3)6,  Mn(NO3)2,  Co(NO3)2,  Zn(NO3)2, 
or  Ni(NO3)2+Aq;  insol.  or  exceedingly  si. 
sol.  in  Pb(NO3)2H-Aq.  (Mulder.) 

Imperfectly  sol.  in  AgNO3+Aq.  (Wacken- 
roder;) 

Cone.  AgNO3+Aq  dissolves  AgCl  per- 
ceptibly. 

Less  sol.  in  AgNO3+Aq  than  AgBr.  (Risse, 
A.  111.  39.) 

Solubility  in  0.02N  AgNO3+Aq  =  0.15X 
10 -7  g.  mols.  per  1.  (Bottger.) 

100  ccm.  of  3-N  solution  of  AgNO3  dis- 
solve 0.08  g.  AgCl  at  25°.  More  dil.  solutions 
dissolve  very  slight  amounts  of  AgCl.  (Hell- 
wig,  Z.  anorg.  1900,  25.  177.) 

Solubility  in  2-N  AgNO3+Aq  at  ord. 
temp.  =  0.03  X10-3  g.  equiv.  AgCl.  (Forbes, 
J.  Am.  Chem.  Soc.  1912,  33.  1946.) 


Solubility  in  AgNO3+Aq  at  t°. 
(Det.  by  volumetric  method.) 

AgN03:H20=2:l 


G.  AgN03 

n/10  NaCl 

t° 

g.  AgCl  re- 
tained per  100 

ccm. 

g.  AgNO" 

6 

2 

57 

0.478 

7 

2 

45 

0.410 

8 

2 

40 

0.359 

9 

2 

35 

0.319 

11 

2 

30 

0.261 

7 

1 

26 

0.205 

10 

1 

22 

0.143 

10 

4 

65 

0.572 

10 

5 

86 

0.715 

828 


SILVER  CHLORIDE 


Solubility  in  AgNO3+Aq  at  t°.  —  Continued. 

heim  and  Steinhauser,   Z.   anprg.    1900,   25. 
103.) 

Solubility  in  Na  thiosulphate  +Aq  at  16°. 

AgNO3:H2O=l 

i 

5 
6 
7 
8 
9 
5.5 
6.5 
12 

1 
1 
1 
1 
1 
0.5 
0.5 
0.5 

94 
84 
75 
66 
58 
48 
40 
23 

0.286 
0.239 
0.205 
0.  179 
0.159 
0.130 
0.110 
0.060 

g.  dissolved  AgCl 
g   Na-S-Hj  *H»n 

in  100  cc.  water         experimental 

calculated 

2.08                  0.29 
4.16                  0.64 
6.24                  0.88 
8.35                   1.26 
16.70                  2.54 
20.83                   3.28 

0.80 

1.60 
2.40 
3.21 
6.42 
7.99 

AgN03:H20=l 

:2 

6 

7 
8 
10 
12 
8 
12 

0.5 

0.5 
0.5 
0.5 
0.5 
0.25 
0.25 

104 
92 

85 
73 
61 
45 

28 

0.120 
0.103 
0.090 
0.072 
0.060 
0.045 
0.030 

(Abney,  Z.  phys.  Ch.  1895,  18.  65.) 

A  solution  of  Na2S2O3+Aq  containing  200 
g.  Na2S2O3  per  liter,  dissolves  0.454  g.  AgCl 
per  g.  of  Na2S2O3  at  35°.     (Richards  and 
Faber,  Am.  Ch.  J.  1899,  2J.  170.) 

Solubility  in  salts  +Aq. 

(Lowry,  Roy,  Soc.  Proc.  1914,  91.  A,  58.) 

Solubility  in  AgNO3+Aq  at  20°. 
(Det.  by  gravimetric  method.) 

Solvent 

% 
Cone. 

Grams  AgCl 
sol.  in  100 
grams  solvent 

g.  AgNOs                g.  H2O 

g.  AgCl  retained 
per  100  g.  AgNOs 

Sodium  thiosulphate 

Ammonium  thiosulphate 

Sodium  sulphite 

Ammonium  sulphite 
carbonate 
Ammonia  +  Aq 

Magnesium  chloride 
Potassium  cyanide 
Ammonium  sulphocyanide 

Potassium           ' 
Calcium 
Barium 
Aluminum 
Thiocarbamide     - 
Thiosinamine 

1 

'   5 
10 
20 
1 
5 
10 
10 
20 
10 
10 
3 
15 
50 
5 
5 
10 
15 
10 
10 
10 
10 
10 
1 
5 
10 

0.40 
2.00 
4.10 
6.10 
0.57 
1.32 
3.92> 
0.44' 
0.95 
Trace 
0.05 
1.40 
7.58 
0.50 
2.75, 
0.08 
0.54 
2.88, 

o.ir 

0.15 
0.20 
2.02 
0.83 
0.40 
1.90 
3.90 

20° 

25° 

20° 

,25° 

220 
220 
220 
220 
220 

110 
165 
220 
330 
440 

0.1372 
0.1009 
0.0722 
0.0402 
0.0294 

(Lowry,  Roy.  Soc.  Proc.  1914,  91.  A,  56.) 
Insol.  in  Na2SO4+Aq. 

Solubility  of  AgCl  in  Na2SO3+Aq  at  25°. 
G.  formula  weights  per  1. 

8Oi 

Ag 

SOs 

Ag 

0.080 
0.106 
0.220 
0.234 

0.478* 

0.011 
0.017 
0.033 
0.036 
0.057* 

0.483* 
0.470 
0.652 
0.890 
0.937 

0.059* 
0.070 
0.103 
0.140 
0.142 

*  In  presence  of  0.05  Cl. 
(Luther  and  Leubner,  Z.  anorg.  1912,  74.  393.) 

Easily  sol.  in  Na2S2O3  or  KCN+Aq. 

When  freshly  pptd.,  very  sol.  in  solutions 
of  soluble  thiosulphates,  and  especially  in  cone 
Na2S2O3+Aq,  which  dissolves  AgCl  almost 
as  readily  as  H2O  dissolves  sugar.  K2S2O3  + 
Aq,  even  when  very  dil.,  also  dissolves  AgCl; 
also  SrS2O3-f  Aq.  (Herschel,  1819.) 

Sol.  in  KAsO2+Aq.    (Reynoso.) 

Cold  NaHSO3+Aq  dissolves  a  consider- 
able amount  of  AgCl.  (Rosenheim  and  Stein- 
hauser, Z.  anorg.  1900,  25.  78.) 

Sol.  in  cold  sat.  (NH4)2S2O3+Aq.    (Rosen- 


(Valenta,  M.  1894,  15.  250.) 

Solubility  in  salts +Aq. 

31.71  cc.  of  a  solution  of.  sodium  thiosul- 
phate containing  31.869  g.  Na2S2O3  per  liter 
(i.  e.  5  g.  of  the  hydrate  in  100  cc.  of  the  solu- 
tion) dissolve  0.6124  g.  AgCl. 

21.88  cc.  of  a  solution  of  ammonium  thio- 
sulphate containing  50  g.  (NH4)2S2O3  per 
liter  dissolve  0.7024  g.  AgCl. 

27.34  cc.  of  a  solution  of  potassium  cyanide 
containing  49.511  g.  KCN  per  liter  dissolve 


SILVER  CHLORIDE 


1.4926  g.  AgCl.  (Cohn,  Z.  phys\  Ch.  1895, 
18.  63.) 

Solubility  of  AgCl  in  sodium  thiosulphate 
and  potassium  cyanide  solutions  may  be  de- 
termined without  reference  to  experimental 
date.  (Cohn.) 

SI.  sol.  in  liquid  NH3.  (Franklin.  Am.  Ch. 
J.  1898,  20.  829.) 

Insol.  in  moderately  dil.  Pb(C2H3O2)2+Aa. 

10  ccm.  normal  Hg(C2H3O2)2+Aq  contain- 
ing 0.1  g.  Hg  dissolve  0.01892  g.  AgCl  at  15°. 
(Stas.) 

100  ccm.  of  a  solution  of  a  mixture  of  Na 
and  Hg  acetates  dissolve  0.00175  g.  AgCl. 
(Stas,  A.  ch.  (5)  3.  145.) 

Only  si.  sol.  in  liquid  NH3. 

Solubility  curve  for  AgCl,  AgCl,  3NH3, 
AgCl,  5NH3.  (Jarry,  A.  ch.  1899,  17.  342.) 

Insol.  in  alcoholic  ammonia.  (Bodlander, 
Z.  phys.  Ch.  1892,  9.  731.) 

Nearly  insol.  in  ether.  (Mylius  and  Hiitt- 
ner,  B.  1911,  44.  1316.) 

Perceptibly  sol.  on  warming  with  solution 
of  tartaric  acid,  but  nearly  the  whole  is  de- 
posited on  cooling. 

Insol.  in  acetone..  (Naumann,  B.  1904,  37. 
4329);  insol.  in  acetone  and  in  methylal. 
(Eidmann,  C.  C.  1899,  II.  1014.) 

Insol.  in  methyl  acetate.  (Bezold,  Dissert. 
1906;  Naumann,  B.  1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Hamers,  Dissert. 
1906;  Naumann,B.  1910,  43.  314.) 

Sol.  in  methylamine+Aq.     (Wurtz,  A.  ch. 


C2H5NH2 

AgCl 

0.01272 
0.03942 
0.05512 
0.06572 
0.10300 

0.000114 
0.000156 
0.000235 
0.000312 
0.000824 

t° 

CsHiNHi 

Ag 

18 

0.094 

0.00458 

25 

0.093 

0.00474 

25 

0.094 

0.00478 

18 

0.236 

0.0132 

25 

0.234 

0.0136 

18 

0.462 

0.0251 

At  25°,  1  1.  methylamine+Aq,  containing 
1.017  g.  mols.  CH3NH2,  dissolves  0.0387  g. 
mol.  AgCl;  0.508  g.  mol.  CH3NH2,  0.0178  g. 
mol.  AgCl.  (Bodlander  and  Eberlein,  B. 
1903,  36.  3948.) 

Solubility  in  ethyamine+Aq  at  25°. 
G.  mols.  per  1. 


(Wuth,  B.  1902,  36.  2416.) 

Solubility  in  ethylamine+Aq  at  t°. 
G.  mols.  per  1. 


(Euler,  B.  1903,  36.  2880.) 


(3)  30.  453.) 
Solubility  of  AgCl  in  methylamine  at  11.5°. 

At  25°,   1  1.  ethylamine+Aq,   containing 
0.483  g.  mol.  C2H6NH2,  dissolves  0.0314  g. 
mols.  AgCl;  0.200  g.  mol.  C2H6NH2,  0.0115  g, 
mol.  AgCl;  0.100  g.  mol.  C2H5NH2,  0.0062  g. 
mol.  AgCl.    (Bodlander  and  Eberlein.) 
Sol.  in  amylamine+Aq,  but  less  than  in 
NH4OH+Aq. 
Sol.  in  caprylamine+Aq. 
Easily  sol.  on  warming  in  ethylene  diamine 
+Aq.     (Kurnakow,  Z.  anorg.  1898,  17.  220.) 
Easily  sol.  in  alcoholic  solution  of  thiaceta- 
mide.    (Kurnakow,  J.  pr.  1895,  (2)  61.  251.) 
Insol.    in    benzonitrile.       (Naumann,    B. 
1914,  47.  1370.) 

Solubility  in  pyridine  at  t°. 

%  CHsNH2 

%  AgCl 

%  CH3NH2       %  AgCl 

1.78 
4.44 
5.51 
7.66 

0.16 
0.62 
0.83 
1.32 

13.70           3.29 
18.69           5.43 
36.69           9.93 

(Jarry,  A.  ch.  1899,  (7)  17.  342.) 

Solubility  in  methylamine+Aq  at  25°. 
G.  mols.  per  1. 

CH3NH2 

AgCl 

0.0200 
0.0400 
0.0740 
0.0947 
0.1950 

0.000300 
0.000370 
0.000424 
0.000447 
0.000481 

t° 

g.  AgCl  sol. 
in  100  g. 
pyridine 

,  Solid  phase 

-52 
-49 
-35 
-30 
-25 

oo 

0.70 
0.77 
0.99 
1.36 
1.80 
2.20 
2175 
3.71 
3.85 
4.35 
5.05 
5.60 

AgCl,  2C5H6N 
AgCl,  C5H5N 

(Wuth,  B.  1902,  35.  2416.) 

Solubility  in  methylamine+Aq  at  t°. 
G.  mols.  perl. 

t° 

CH3NH2 

Ag 

transition  point 
-20 
-18 
-10 
-  5 
-   1 

18 
25 
25 

0.93 
0.93  . 
0.93 

0.0315 
0.0338 
0.0335 

(Euler,  B.  1903,  2 

6.  2880.) 

830 


SILVER  CHLORIDE  AMMONIA 


Solubility  in  pyridine  at  t°.  —  Continued. 

Solubility  of  AgF  in  H2O  at  t°. 

Gr-kor   1  HO  o-     TT  O 

g   AgCl  sol 

t°      . 

in  100  g. 

Solid  phase 

t° 

AgF 

Solid  phase 

pyridine 

-14.2 

+18.5 
18.65 

60 
165 
169.5 

Ice+AgF,  4H2O 
AgF,  4H20 
"  +AgF,  2H20 

transition  point 
0 
10 

5^35 

Q     17 

' 

20 
30 

1.91 
1.20 

20 
24 

OK 

172 
178 

17Q    ^ 

.AgF,a2H20 

40 

0.80 

28.5 

215 

ft 

50 
60 
70 
80 

0.53 
0.403 
0.32 
0.25 

AgCl 

32 
39.5 
108 

193 
222 
205 

AgF,2H2O+AgF 
AgF 

90 

0.22 

(Guntz,  A.  ch.  1914,  (9)  2.  101.) 

100 

0  18 

110 

0.12 

Sp.  gr.  AgF+Aq  at  18°. 

(Kahlenberg,  J.  phys.  Chem.  1909,  13.  423.) 

%  AgF 

Sp.  gr. 

Easily  sol.  in  warm  piperidine.     (Varet, 
C.  R.  1892,  115.  335.) 
Mol.  wt.  determined  in  piperidine.     (Wer- 
ner, Z.  anorg.  1897,  15.  16.) 
Quinoline  dissolves  traces  of  AgCl.    (Varet, 

7.20 
29.60 
4Q.20 
56.40 
66.20 

1.07 
1.38 
1.82 
2.  OP 
2.62 

As  sol.  in  coniine+Aq  as  in  NH4OH+Aq. 
(Blyth,  Chem.  Soc.  1.  350.) 

Sol.  in  sinamine,  and  thiosinamine+Aq. 
Min.     Cerargyrite. 

Silver  chloride  ammonia,  AgCl,  2NH3. 

Decomp.  by  H2O.  (Terreil,  A.  Phys. 
Beibl.  7.  149.) 

2AgCl,  3NH3.  Decomp.  on  air  and  in  H2O 
to  AgCl.  Sol.  in  cone.  NH4OH+Aq,  from 
which  it  can  be  crystallised.  (Rose.) 

Insol.  in  alcohol.  (Bodlander,  Z.  phys.  Ch. 
9.  730.) 

AgCl,  3NH3.  More  easily  decomp.  than 
2AgCl,  3NH3. 

SI.  sol.  in  liquid  NH3.  (Jarry,  A.  ch.  1899, 
(7)  17.  343.) 

AgCl,  5NH3.  SI.  sol.  in  liquid  NH3. 
(Jarry,  A.  ch.  1899,  (7)  17.  336.) 

Silver  chlorobromoiodides. 

(Rodwell,  Proc.  Roy.  Soc.  25.  292.) 

Silver  s?/6fluoride  (argentous  fluoride),  Ag2F. 

Decomp.    by   H2O    into   Ag    and   AgF. 
(Guntz,  C.  R.  110.  1337.) 

Decomp.  by  H2O. 

Insol.  in  abs.  alcohol,  ether,  acetone  and 
xylene.  (Wohler  and  Rodewald,  Z.  anorg. 
1909,  61.  63.) 

Decomp.  by  H2O  until  the  solution  con- 
tains 64.5%  AgF,  independent  of  temp. 
(Guntz,  C.  R.  1913,  157.  981.) 

Silver  fluoride,  AgF. 

Extremely  deliquescent.     (Gore.) 

Sol.  in  0.55  pt.  H2O  at  15.5°  with  evolution 

of  heat.     Sp.  gr.  of  sat.  solution  at  15.5°  = 

2.61.    (Gore.) 


(Guntz,  A.  ch.  1914,  (9)  2.  104.) 

Data  on  solubility  of  AgF  in  HF+Aq  are 
given  by  Guntz  (I.  c.). 

SI.  sol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  829.) 

+H2O.  Deliquescent.  Sol.  in  H2O. 
(Guntz,  A.  ch.  1914,  (9)  2.  101.) 

+2H2O.  Deliquescent.  Sol.  in  H2O. 
(Guntz.) 

+4H2O.  Not  deliquescent.  Sol.  in  H2O. 
(Guntz.) 

+5/a  H2O.  Unstable  in  the  presence  of 
crystals  of  AgF+2H2O.  (Guntz,  A.  ch.  1914, 
(9)  2.  101.) 

Silver  hydrogen  fluoride,  AgF,  HF. 
(Guntz.) 

AgF.  3HF.     Very  unstable. 

Sol.  in  HF.     (Guntz,  Bull.  Soc.  1895,  (3) 
13.  114.) 
Silver  stannic  fluoride. 

See  Fluostannate,  silver. 
Silver  tungstyl  fluoride. 

See  Fluoxtungstate,  silver. 
Silver,  fulminating. 

See  Silver  nitride. 
Silver  hydride,  AgH. 

Not  decomp.  by  H2O.    (Bartlett,  Am.  Ch. 
J.  1896,  19.  52.) 
Argentous  hydroxide,  Ag4O2H2. 

Sol.    in   H2O.      Known   only   in   solution. 
(Weltzein,  A.  142.  105.) 
Silver  hydroxide,  AgOH. 

Decomp.  into  Ag2O  and  H2O  above  -40°. 

See  Silver  oxide. 


SILVER  IODIDE 


831 


Argentous  iodide,  Ag2I. 
(Guntz,  C.  R.  112.  861.) 

Silver    imidosulphamide,    AgN(SO2NH2)2  + 


Decomp.  slowly  in  the  air.  Somewhat  sol. 
in  hot,  more  sol.  in  boiling  H2O,  from  which 
it  cryst.  unchanged  on  cooling.  In  aqueous 
solution  is  stable  toward  alkali.  Decomp. 
by  acids.  Difficultly  sol.  in  dry  pyridine; 
easily  sol.  in  pyridine +Aq.  (Hantzsch,  B. 
1905,  38.  1035.) 

'(SO2)3N6H6Ag3+5^H2O.  Nearly  insol. 
in  hot  H2O.  (Ephraim  and  Michel,  B.  1909, 
42.  3845.) 

(SO2)4N7H8Ag5+4H2O.  (Ephraim  and 
Michel.) 

(SO2)4N5HAg6  +  l^,  11,  and  28  H2O. 

Easily  sol.  in  HNO3  and  NH4OH+Aq. 
SI.  sol.  in  pyridine.  Very  sol.  in  pyridine  con- 
taining pyridine  nitrate  and  can^be  recryst. 
therefrom.  (Ephraim  and  Michel.) 

(SO2)4N6Ag7+8H2O.  (Ephraim  and 
Michel.) 

Silver  iodide,  Agl. 

Insol.  in  H2O. 

Calculated  from  electrical  conductivity  of 
Agl+Aq,  Agl  is  sol.  in  1,074,040  pts.  H2O 
at  28.4°,  and  420,  260  pts.  at  40°.  (Holleman, 
Z.  phys.  Ch.  12.  130.) 

1  1.  H2O  dissolves  0.1  mg.  Agl  at  18°. 
(Kohlrausch  and  Rose,  Z.  phys.  Ch.  12.  241.) 

Solubility  in  H2O  =  1  X 1Q-8N.    (Rolla.) 

Solubility  in  H2O  =  0.97  X 1Q-8  g.  mols.  per  1. 
at  25°.  (Goodwin,  Z.  phys.  Ch.  1894, 13.  645.) 

Solubility  of  Agl  in  H2O  at  25°  is  1.05  X10-8 
(in  normality) .  (Thiel,  Z.  anorg.  1900,  24. 57.) 

A  sat.  aq.  solution  at  20.8°  contains  0.0020 
X10-6  g.  equiv.  perl.  (Kohlrausch,  C.  C. 
1901,  II.  1299.) 

1  1.  H2O  dissolves  0.0035  mg.  Agl  at  21°. 
(Kohlrausch,  Z.  phys.  Ch.  1904,  50.  356  ) 

11.  H2O  dissolves  0.00253  mg.  Agl  at  60° 
(Sammet,  Z.  phys.  Ch.  1905,  53.  644.) 

Solubility  in  H2O  =  1.23X10-8  g.-mol 
per  litre  at  25°.  (A.  E.  Hill,  J.  Am.  Chem 
Soc.  1908,  30.  74.) 

0.003  mg.  are  contained  in  1  1.  of  sat.  solu- 
tion at  21°.  (Kohlrausch,  Z.  phys.  Ch.  1908, 

Insol.  in  dil.  HNO3+Aq  or  H3PO4+Aq. 
Decomp.  by  hot.  cone.  HNO3+Aq  or  H2SO4. 
Easily  sol.  in  cone.  HI+Aq. 

1  pt.  Agl  dissolves  in  2510  pts.  NH4OH  + 
Aq  of  0.96  sp.  gr.  (Martini,  Schw.  J.  66.  154)  ; 
in  24£3  pts.  of  0.89  sp.  gr.  (Wallace  and  La- 
mont,  Ch.  Gaz.  1859.  137). 

1  g.  Agl  dissolves  in  26,300  g.  10% 
NH4OH+Aq  (sp.  gr.=0.96)  at  12°.  Insol. 
in  5%  NH4OH+Aq.  (Longi,  Gazz.  ch.  it.  13. 
87.) 

Coefficient  of  solubility  in  NH4OH+Aq 
(density,  0.926)  is  found  lower  than  previ- 
ously obtained  and  of  the  order  of  Veoooo  at 
16°.  (Baubigny,  Bull.  Soc.  1908,  (4)  3.  772  ) 


According  to  Field,  insol.  in  cold  cone.  KC1 
or  NaCl+Aq,  and  only  in  traces  on  boiling, 
and  separates  out  on  cooling. 

100  g.  NaCl  in  cone.  NaCl+Aq  dissolve 
0.95  mg.  Agl  at  15°;  100  g.  NH4C1  in  cone. 
NH4Cl+Aq  dissolve  2.9  mg.  Agl  at  15°;  95  g. 
NaCl +  10  g.  KBr  in  cone,  solution  dissolve 
1.2  mg.  Agl  at  15°;  IOC  g.  KBr+225  g.  H2O 
dissolve  430  mg.  Agl  at  15°;  100  g.  KBr  in 
cone.  KBr+Aq  dissolve  525  mg.  Agl  at  15°; 
100  g.  KI+69  g.  H2O  dissolve  89.8  g.  Agl  at 
15°;  100  g.  KI+92  g.  H2O  dissolve  54.0  g. 
Agl  at  15°;  100  g.  KI+366  g.  H2O  dissolve 
7.25  g.  Agl  at  15.°  (Schierholz,  W.  A.  B. 
101,  2b.  4.) 

Sol.  in  cone.  KI+Aq,  from  which  it  is  pre- 
cipitated by  H2O.  (Field,  C.  N.  3.  17.) 

KI  gives  a  ppt.  with  AgNO3  in  presence  of 
30,000  pts.  H2O.  (Harting.) 

Solubility  in  KI+Aq  at  15°. 


%KI 

%  Agl 

%KI 

%  Agl 

59.16 

53.13 

33.3 

7.33 

57.15 

40 

25.0 

2.75 

50.0 

25.0 

21.74 

1.576 

40.0 

13.0 

20 

0.80 

(Schierholz,   W.   A.   B.    1890,   101.  2b.    10.) 

Solubility  in  KI+Aq  at  25°.   ' 

Mol.  KI  per  1. 

g.  Agl 

perl. 

1.937 

46. 

42 

1.6304 

24. 

01 

1.482 

15. 

46 

1.406 

12. 

55 

1.018 

3. 

47 

1.008- 

3. 

32 

0.734 

1. 

032 

0.586 

0. 

512 

0.335      ' 

0. 

0853 

Hellwig,  Z.  anorg.  1900,  25. 

180.) 

Solubility  in  KI+Aq. 

t=50° 

%  Agl 

%KI 

Solid 

phase 

2.5 

24.8 

Agl 

16.0 

33.8 

' 

28.0 

36.7 

' 

39.0 

38.1 

( 

51.8 

36.2 

' 

53.5 

36.5 

1 

53.5 

36.6 

Agl+. 

\gl,  KI 

53.5 

37.1 

Ag] 

,KI 

53.4 

37.6 

KI+AgI,  KI 

50.4 

40.2 

KI 

45.0 

43.2 

a 

38.0 

47.1 

n 

22.8 

55.5 

a 

10.7 

59.1 

a 

832 


SILVER  IODIDE 


t=30° 


%  Agl 

%  KI 

Solid  phase 

0.1 

10.2 

Agl 

10.0 

31.4 

29.4 

37.6 

a 

42.8 

38.8 

i(  . 

49.7 
49.6 

38.6 
39.5 

Agl  +  Agl,  2KI 
Agl,  2KI 

47.7 

40.9 

a 

46.3 

41.4 

(t 

44.1 

43.2 

Agl,  2KI+KI 

42.8 

43.9 

KI 

35.8 

46.9 

K 

16.0 

55.5 

(( 

0 

60.35 

it 

t=0° 


%  A¥I 

%  KI 

Solid  phase 

0.2 

9.8 

Agl 

1.5 

20.5 

6.5 

26.1 

" 

26.6 

34.6 

!  " 

28.1 

36".  4 

I  n 

38.0 
37.9 

41.3 
42.0 

Agl  +  Agl,  KI 
Agl,  KI 

37.6 

42.7 

u 

37.9 

44.0 

Agl,  KI+KI 

31.3 

46.6 

KI 

21.7 

50.5 

u 

18.0 

51.2 

ii 

9.0 

53.0 

11 

0 

56.1 

<< 

27.5 

48.7 

Agl,  2KI+KI 

21.0 

50.3 

Agl,  2KI 

(Van  Dam  and  Donk,  Chem.  Weekbl.  1911, 

8.  848.) 

Very  sol.  in  KI3+Aq.  (Muth,  Dissert.  1895.) 
Very  sol.  in  H2O  in  presence'of  Nal.  (Kur- 

nakow,  Ch.  Z.  1900,  24.  60.) 

Solubility  in  Al  -f  Aq  at  15°. 


Traces  are  dissolved  by  alkali  nitrates  +Aq. 
Easily  sol.  in  hot  KOH  +Aq,  from  which  it  is 
aptd.  by  H2O  or  alcohol.     Not  decomp;  by 
boiling  KOH+Aq.     (Vogel>  N.  Rep.  Pharm. 

20.  129.) 

100  pts.  of  AgNO3+Aq  sat.  at  11°  dissolve 
2,3  pts.  Agl  in  the  cold,  and  12.3  pts.  on  boil- 
ing.    (Schnauss.) 

Solubility  of  Agl  in  AgNO3+Aq  at  25°. 

Mol.  AgNOs 
in  1  1. 

g.  Agl  in  1  1. 

Solid  phase 

0.20 

0.0680 

\ 

0.25 

0.080 

0.30 

0.090 

0.35 

0.125 

0.40 

0.167 

0.45 

0.224 

Agl 

0.50 

0.299 

0.55 

0.400 

0.60 

.0.528 

0.65 

0.672 

0.70 

0.850 

1.215 

3.08 

1 

1.63 

6.26 

Ag2IN03 

2.04 

10.90 

J 

2.54 

16.1 

3.115 

22.7 

3.75 
4.055 

33.2 
40.0 

.Ag3I(N03)2 

4.69 

53.2 

5.90 

85.0 

/'HWIl^r;™-    *7    r,«™.rr     1  OHO    QK     171   ^ 

Composition  of  the  sat. 

solution  in  mols.  per 
1000  mols.  H2O 

Solid  phase 

Mols. 

Mols. 

Na2I2 

A««Ii 

35.63 

8.14 

Agl 

40.54 

10.94 

a 

61.55 

25.15 

" 

80.55 

38.19 

tl 

94.25 

47.79 

t( 

107.52 
117.96 

57.52 
51.70 

Agl+AgI,  Nal,  3^H20 
Agl,  Nal,  3^H2O 

134.40 

46.82 

u 

135.83 

46.36 

AgI,NaI,3^H2O+NaI 

133.81 

43.03 

Nal 

129.02 

34.85 

• 

122.56 

22.82 

• 

117.11 

11.93 

u 

111.52 

lt 

(Krym,  J.  Russ.  Phys.  Chem.  Soc.  1909,  41. 

382.) 

Solubility  of  Agl  in  25%  AgNO3+Aq 
reaches  a  maximum  at  about  60°  and  at  the 
point  of  maximum  solubility  the  quantity 
dissolved  amounts  to  about  5  g.  Agl  per  100 
g.  AgN03.  (Lowry,  Roy.  Soc.  Proc.  1914, 
91,  A,  66.) 

Sol.  in  hot  Hg(NO3)2+Aq,  from  which 
it  crystallizes  on  cooling. 

Solubility  of  Agl  in  Hg(N03)2+Aq  at  25°. 


Mols. 
Hg(N03)2 
perl. 

g.  Agl 
perl. 

Mols. 
Hg(NOs)8 
per  1. 

g.  Agl 
per  1. 

0.010 
0.0125 
0.025 

0.800 
0.841 
1.118 

0.050 
0.100 
1.000 

1.737 
2.730 
25.160 

Solubility  is  not  affected  by  presence  of 
0.1to2NHNO3. 

(Morse,  Z.  phys.  Ch.  1902,  41.  708.) 

Sol.  inKCN+Aq. 

SI.  sol.  in  Na2S2O3+Aq  when  suspended  in 
much  H2O,  but  separates  again  on  addition  of 
KI+Aq.  (Field.) 

Insol.  in  Na2S2O3+Aq.  fFogh,  C.  R. 
1890,  110.  711.) 


SILVER  OXIDE 


833 


Solubility  in  salts+Aq. 

2AgI,    NH3.      (Rammelsberg,    Pogg.    48. 

17O  "> 

Solvent 

% 
Cone. 

grams  Agl  sol. 
in  100  grams 
solvent 

1  i  \j.) 

Composition  is  Agl,  NH3.     (Longi,  Gazz. 
ch.  it.  13.  86.) 

Sol.  in  liquid  NH3.    (Jarry,  A.  ch.  1899,  (7) 

Sodium  thiosulphate 

1 

0.03 

17.  371.) 

"             "         " 

5 

0.15 

Agl,  2NH3.    (Terreil,  C.  R.  98.  1279.) 

"             "         " 

10 

0.30 

20 

"              "         " 

15 

0.40 

Silver  nitride,  Ag3N. 

Sodium  sulphite 

Ammonium  sulphite 
Potassium  cyanide 

20 
10 
20 
10 
5 

0.60 
0.01 
0.02 
Traces 

8.23 

25 

Berthollet's  "knallsilber."    Very  explosive. 
Insol.  in  H2O.     Sol.  in  KCN+Aq.     Slowly 
sol.  in  NH4OH+Aq.     (Raschig,  A.  233.  93.) 
(Angeli,  Chem.  Soc.  1894,  66.  (2)  93.)  " 

Ammonium  sulphocyanide 

5 
i  n 

0.02' 
One 

on 

Argentous  oxide,  Ag4O. 

«. 

1U 

1  *» 

.u» 

010 

&\j 

Insol.   in  H2O.     Decomp.   by  acids  into 

Potassium         ' 

J.O 

10 

.  JLO 

argentic  oxide  and  silver.    Insol.  in  NH4OH  + 

Calcium            ' 

-LU 

10 

0.03 

• 

Aq  or  HC2H3O2.     (v.  der  Pfordten,  B.  20. 

Barium              ' 

10 

009 

1458.) 

Aluminum        ' 

-LU 

10 

.  V  /  w 

0.02 

Contains  H,  and  is  a  hydroxide  Ag4,H2O. 

Thiocarbamide 

10 

0  7Q 

25 

(v.  der  Pfordten,  B.  21.  2288.) 

Thiosinamine 

AVF 
1 

\J  •   4.  t7 

0  008 

The  above  substance  is  a  mixture,  accord- 

-L 

5 

\J  .  Uv/O 

0.05 

ing  to  Friedheim  (B.  20.  2557.) 

10 

0.09 

Silver  oxide,  Ag2O. 

(Valenta,  M.  1894,  15.  250.) 

Very  sol.  in  liquid  NH3.  (Franklin,  Am. 
Ch.  J.  1898,  20.  829;  Jarry,  A.  ch.  1899,  (7) 
17.  370.) 

Easily  sol.  in  liquid  NH3.    (Ruff  and  Geisel, 

B.  1905,  38.  2662.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II,  1014);  (Naumann,  B.  1904,  37.  4329.) 

Insol.  in  methyl  acetate.  (Bezold,  Dis- 
sert. 1906);  (Naumann,  B.  1909,  42.  3790.) 

Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.  257.) 

Much  less  sol.  in  hot  alcoholic  thiourea  than 
AgCl  and  AgBr.  (Reynolds,  Chem.  Soc. 
1892,  61.  253.) 

Insol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1370.) 

Slowly  sol.  in  piperidine  at  100°.     (Varet, 

C.  R.  1892,  115.336.) 

0.10  pts.  is  sol.  in  100  pts.  pyrioline  at  10°. 

8.60  pts.  are  sol.  in  100  pts.  pyridine  at  121°. 
(Laszczynski,  B.  1894,  27.  2288.) 

Mol.  wt.  determined  in  piperidine.  (Wer- 
ner, Z.  anorg.  1897,  15.  16.) 

Min.  lodyrite. 

Silver  hydrogen  iodide,  3AgI,  HI+7H2O.    . 
(Berthelot,  C.  R.  91.  1024.) 

Silver  sodium  iodide,  2AgI,  Nal. 

Very  sol.  in  acetone.  (Marsh,  Chem.  Soc. 
1913,  103.  784.) 

Agl,  NaI+3^H2O.  (Krym,  J.  Russ. 
Phys.  Chem.  Soc.  1909,  41.  382.) 

See  Agl+Nal  under  Agl. 

Silver  iodide  ammonia,  Agl,  NH3. 

Sol.  in  liquid  NH3.  (Jarry,  A.  ch.  1899, 
7)  17.  371.) 


Somewhat  sol.  in  H2O.    (Bucholz.) 

Sol.  in  3000  pts.  H2O.  (Bineau,  C.  R.  41.  509) ; 
sol.  in  96  pts.  H2O.  (Abl.) 

Sol.  in  15,360  pts.  H2O.  (Levi,  Gazz.  ch.  it. 
1901,  31.  (1)  1.) 

Solubility  in  H2O  at  25°  =  2.16X10-4  mols. 
AgOH  per  litre.  (Noyes,  J.  Am.  Chem. 
Soc.  1902,  24.  1147.) 

1  liter  sat.  aqueous  solution  at  19.96°  con- 
tains 2.14X10-2  g.;  at  24.94°  contains  2.5  X 
10  2  g.  Ag2O.  (Bottger,  Z.  phys.  Ch.  1903, 

1  1.  H2O  at  25°  dissolves  1.8X10-4  gram- 
atoms  of  silver.  Determined  from  its  solu- 
bility in  NH3.  (Abegg  and  Cox,  Z.  phys. 
Ch.  1903,  46.  11.) 

1  1.  H2O  dissolves  C.0215  g.  Ag2O  at  20°. 
(Whitby,  Z.  anorg.  ]910,  67.  108.) 

The  solubility  of  Ag2O  in  H2O  varies  with 
the  method  of  preparation. 

Solubility  of  Ag2O  (prepared  by  action  of 
NaOH,  freshly  prepared  by  the  solution  of 
Na  in  H2O,  on  a  dil.  solution  of.AgNO3)  = 
2.16X10-4  g-mol.  in  1  1.  H2O  at  25°;  2.97  X 
10-4g.-mol.  at  50°. 

Solubility  of  Ag2O  (prepared  by  action  of 
aqueous  barium  hydroxide  on  AgNO8)  = 
2.23  X10-4  g.-mol.  in  1  1.  H2O  at  25°; 
3. 09X1<>4  g.-mol.  in  1  1.  H2O  at  50°. 

Solubility  of  Ag2O  (prepared  by  action  of 
cone.  NaOH+Aq  on  moist,  freshly  pptd. 
AgCl)=2.32X10-4  g.-mol.  in  1  1.  H2O  at 
25°;  3.55  X10-4  g.-mol.  at  50°. 

Solubility  of  Ag2O  (prepared  by  action  of 
cone.  NaOH+Aq.  on  moist,  freshly  pptd. 
Ag2CO3)=2.95X10-4  g.-mol.  in  1  1.  H2O  at 
25°;  3.89  X10-4  g.-mol.  at  50°.  (Rebiere, 
Bull.  Soc.  1915,  (4)  7.  311.) 

Sol.  in  acids.  NH4OH,  and  (NH4)2CO3-t 
Aq.  Decomp.  by  alkali  chlorides,  bromides,, 


834 


SILVER  OXIDE 


and  iodides +Aq.  Sol.  in  alkali  cyanides,  and 
thiosulphates+Aq.  SI.  sol.  in  nitrates +Aq; 
insol.  in  sulphates +Aq.  When  freshly 
pptd.,  sol.  in  NH4SCN+Aq.  SI.  sol.  in 
NH4NO3+Aq.  Abundantly  sol.  in  Ba(NO3)2 
+Aq  without  pptn.  of  Ba02H2.  Sol.  in 
boiling  Mn(NO3)2,  Ni(NO3)2,  Co(NO3)2, 
Cu(NO3)2,  and  Ce2(NO3)6+Aq  with  pptn. 
of  oxides.  (Persoz.) 

Insol.  in  KOH,  and  NaOH+Aq.    SI.  sol. 
in  BaO2H2+Aq.    (Berzelius  (?). 

SolubiHty  in  NH4OH+Aq  at  25°. 


G.  at.  Ag  per  1. 

Mol.  NH3  per  1. 

0.0654 

0.214 

0.0658 

0.220 

0.134 

0.458 

0.140 

0.469 

0.205 

0.671 

0.205 

0.684 

0.225 

0.720 

0.224 

0.733 

0.251 

0.811 

0.248 

0.827 

0.242 

0.830 

0.257 

0.876 

0.278 

0.899 

0.276 

0.915 

0.299 

0.999 

0.343 

1.147 

0.454 

1.498 

0.470 

1.522 

(Whitney  and  Melcher,  J.  Am.  Chem.  Soc. 
1903,  25.  78.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  ch. 
J.  1898,  20.  829.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014);  (Naumann,  B.  1904,  37.  4329.) 

Insol.  in  ethyl  acetate.  (Hamers,  Dissert. 
1906;  Naumann,  B.  1910,  43.  314.) 

SI.  sol.  in  amylamine+Aq,  easily  in 
methylamine+Aq  fWurtz,  A.  ch.  30.  453); 
also  in  ethylamine,,and  thiosinamine+Aq. 

Solubility  in  methylamine+Aq.  at  18°. 
G.  mols.  per  1. 


CH3NH2 

Ag 

0.1 

0.5 
1.0 

0.0221 
0.118 
0.228 

(Euler,  B.  1903,  36.  2879.) 

Solubility  in  ethylamine+Aq  at  18°. 
G.  mols.  per  1. 

C2H6NH2 

Ag 

0.1 
0.5  (interpolated) 
1.0            " 
0.561 
0.927 

0.0322 
0.160 
0.314 
0.180 
0.291 

(Euler.) 

Silver  peroxide,  Ag2O2. 

Sol.  in  cone.  H2SO4  (Rose),  and  in  pure 
HNO3  +Aq  without  decomp.  Sol.  in  NH4OH 
+Aq.  (Schonbein,  J.  pr.  41.  321.) 

Sol.  in  HNO3  and  H2SO4  with  decomp. 
Mulder,  R.  t.  c.  1898,  17.  151.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  829.) 

Silver  oxide  ammonia. 
See  Silver  nitride. 

Silver  oxybromide,  Ag7OBr7. 

Insol.  in  H2O.  Insol.  in  HNO3.  Sol.  in 
lot  ammonia  and  in  NaOCl  +  Aq.  f  Seyewetz, 
~.  R.  1912,  154.  357.) 

Silver  oxyfluoride,  AgF,  AgOH. 

Decomp.  by  H2O  with  separation  of  Ag2O. 
(Pfaundler.) 

Silver  pei  oxyfluoride,  2Ag3O4,  AgF. 
(Tanatar,  Z.  anorg.  1901,  28.  335.) 
4Ag3O4,  3AgF.     (Tanatar,  Z.  anorg.  1901, 

28.  335.) 

Silver  oxyiodide,  Ag2O,  Agsly. 

(Seyewitz,  Bull.  Soc.  1894,  (3)  11.  452.) 

Silver  phosphide,  AgP2. 

Sol.  in  HNO3.  Attacked  by  aqua  regia. 
(Granger,  C.  R.  1897,  124.  897.) 

Ag4P6.  Insol.  in  HCl+Aq;  easily  sol.  in 
HNOa+Aq.  (Schrotter,  J.  B.  1849.  247.) 

Ag2P5.    (Hackspill,  C.  R.  1913,  157.  720.) 

Ag3P  (?).  (Fresenius  and  Neubauer,  Z. 
anal.  1.  340.) 

Silver  phosphoselenide,  Ag2Se,  P2Se. 

Insol.  in  H2O  or  HCl+Aq.  Sol.inHNO3+ 
Aq.  Insol.  in  cold,  decomp.  by  hot  alkalies  + 
Aq;  (Hahn,  J.  pr.  93.  436.) 

2Ag2Se,  P2Se3.  Insol.  in  H2O,  HC1,  or 
HNO3+Aq;  slowly  sol.  in  red  fuming  HNO3. 
(Hahn,  J.  pr.  93.  440.) 

2Ag2Se,  P2Se5.  Sol.  only  in  fuming  HNO3. 
(Hahn.) 

Silver  phosphosulphide,  2Ag2S,  P2S. 

Ag2S,  P2S.    (Berzelius,  A.  46.  254.) 

2Ag2S,  P2S3.  Easily  sol.  in  HNO3+Aq 
without  separation  of  P.  (Berzelius.) 

Ag4P2S7.    (Berzelius.) 

Ag4PS3.  Easily  attacked  by  hot  cone. 
HC1.  SI.  decomp.  Insol.  in  hot  HNO3.  De- 
comp. by  aqua  regia.  (Ferrand.  A.  ch.  1899. 
(7)  17.  413.) 

Silver  selenide,  Ag2Se. 

Sol.  in  boiling  HNO3+Aq  as  Ag2SeO3, 
which  separates  out  by  dilution  with  H2O. 
(Berzelius.) 

Insol.  in  Hg2(NO3)2+Aq.  (Wackenroder, 
A.  41.  327.) 


SODIUM  ACETYLIDE  ACETYLENE 


835 


Min.  Naumannite.  Insol.  in  dil.,  but  sol. 
in  cone.  HNO3+Aq. 

Silver  sulphamide  (silver  thionyl  amide). 
SO2(NHAg)2. 

Insol.  in  pyridine.  (Hantzch  and  Holl,  B. 
1901,  34.  3436.) 

+H2O.  (Ephraim  and  Gurevitsch,  B. 
1910,  43.  146.) 

Argentous  sulphide,  Ag4S. 

Easily  sol.  in  warm  dil.  HNO3+Aq,  and  in 
cone.  H2SO4  without  separation  of  S.  Sol.  in 
cone.  KCN+Aq.  '(v.  der  Pfordten,  B.  20. 
1458;  Guntz,  C.  R.  112.  861.) 

Silver  sulphide,  Ag2S. 

Less  sol.  in  H2O  than  Agl.  (Lucas,  Z. 
anorg.  1904,  41.  210.) 

1  1.  H2O  dissolves  about  4X10  n  g.  at.  Ag 
as  Ag2S  at  18°.  (Bernfeld,  Z.  phys.  Ch.  1898. 
26.  72.) 

1  1.  H2O  dissolves  0.8X106  g.  mols.  at 
16-18°.  (Biltz,  Z.  phys.  Ch.  1907,  58.  291.) 

1  1.  H2O  dissolves  0.552  X 10  6  g.  mols. 
Ag2S  at  18°.  (Weigel,  Z.  phys.  Ch.  1907,  58. 
294.) 

Sol.  in  cone.  HNO3+Aq  with  separation 
of  S.  Sol.  in  hot  cone.  HCl+Aq.  Not  de- 
comp.  by  CuCl2+Aq,  but  by  CuCl2+NaCl 
+Aq.  Insol.  in  NH4OH+Aq.  Insol.  in 
H2SO3+Aq,  or  in  Hg(NO3)2+Aq. 

Insol.  in  H2O,  dil.  acids,  alkalies,  and  alkali 
sulphides +Aq.  (Fresenius.) 

Sol.  in  HCN+Aq.  (Hahn,  C.  C.  1870. 
240.) 

Pptd.  Ag2S  is  very  sol.  in  HNO3  containing 
more  than  5%  HNO3.  (Gruener,  J.  Am. 
Chem.  Soc.  1910,  32.  1032.) 

Only  very  si.  sol.  in  AgNO3+Aq,  even  at 
100°.  (Lowry,  Roy.  Soc.  Proc.  1914,  91,  A. 
70.) 

Sol.  in  KCN+Aq.  (Hahn,  C.  C.  1870. 
240.) 

Difficultly  sol.  in  KCN+Aq;  less  difficultly 
if  Ag2S  is  pptd.  from  a  very  dil.  solution. 
Amt.  of  KCN  present  also  has  influence  on 
the  solubility.  Ag2S  dissolved  in  cone.  KCN 
+Aq  separates  out  on  dilution.  (Be"champ, 
J.  pr.  60.  64.) 

Insol.  in  NH4C1  or  NH4NO3+Aq.    (Brett.) 

Min.  Argentite.  Acanthite.  Sol.  in  cone. 
HNO3-f  Aq  with  separation  of  S. 

Sol.  in  citric  acid+Aq  with  addition  of 
KNO3.  (Bolton,  C.  N.  37.  48.) 

Silver  bisulphide,  Ag2S2. 

Sol.  in  H2O  with  decomp.;  also  sol.  with 
decomp.  in  HC1,  HNO3.  CS2  does  not  dissolve 
out  S.  (Hantzsch,  Z.  anorg.  1898,  19.  105.) 

Silver  sodium  sulphide,  3Ag2S,  Na2S+2H2O. 
Sol.  in  cone.  Na2S+Aq  with  decomp.;  sol. 
in  H2O  with  decomp.     (Ditte,  C.  R.  1895, 
120.  93.) 


Silver  zinc  sulphide,  Ag2S,  3ZnS. 
(Schneider,  J.  pr.  (2)  8.  29.) 

Silver    sulphimide*    (silver    thionyl    imide), 

S02NAg. 

Very  si.  sol.  in  cold,  more  sol.  in  hot  H2O. 
Very  sol.  in  dil.  HNO3.  (Traube,  B.  1892, 
25.  2474.) 

Silver  sulphophosphide. 
See  Silver  phosphosulphide. 

Silver  telluride,  Ag2Te. 

Min.  Hessite.    Sol.  in  warm  HNO3-f  Aq. 

Sodammonium,  Na2(NH3)2. 

100  g.  liq.  NH3  dissolve  60.5  g.  at  -23°; 
56.4  g.  at  0°;  56  g.  at  +5°;  55  g.  at  9°.  (Joannis 
A.  ch.  1906,  (8)  7.  41.) 

Sodium,  Na2. 

Violently  decomposes  H2O,  alcohol,  etc. 
Insol.  in  hydrocarbons.  Easily  sol.  in  acids 
with  violent  action. 

Solubility  in  fused  NaOH. 
G.  sol.  in  100  g.  fused  NaOH  at  temp. 


t° 

G.  per  100  g.  NaOH 

480 

25.3 

600 

10.1 

610 

9.9 

670 

9.5 

760 

7.9 

800 

6.9 

(Hevesy,  Z.  Elektrochem.  1909,  15.  531.) 

Insol.  in  liquid  CO2.     (Biichner,  Z.  phys. 
Ch.  1906,  54.  674.) 

Sol.  in  liquid  NH3.     (Franklin,  Am.  Ch.  J. 
1898,  20.  829.) 

1  gram  atom  dissolves: — 

at  +22°  in  6.14  mol.  liquid  NH3. 


0° 
—30° 
—50° 
—70° 
— 105C 


5.87 
5.52 
5.39 
5.20 
4.98 


(Ruff,  B.  1906,  39.  839.) 

%  ccm.  oleic  acid  dissolves  0.0449  g.  Na 
in  6  days.  (Gates,  J.  phys.  Chem.  1911,  15. 
143.) 

Insol.  in  ethylamine  and  in  secondary  and 
tertiary  amines.  (Kraus,  J.  Am.  Chem.  Soc. 
1907,  29.  1561.) 

Sodium  acetylide  acetylene,  Na2C2,  C2H2. 

Very  deliquescent.  Decomp.  by  H2O  and 
by  absolute  alcohol.  Insol.  in  ether,  ligroin, 
etc.  (Moissan,  C.  R.  1898,  127.  915.) 


836 


SODIUM  AMALGAM 


Sodium  amalgam. 
NaHg6.    Stable  in  contact  with  the  liquid 
amalgam  from  0°-40.5°.    Can  be  cryst.  from 
Hg  without  decomp.  at  ^,ny  temp,  between 
these  limits. 
NaHg5.    Stable  in  contact  with  the  liquid 
amalgam   from   40.5°-150°.     Can   be   cryst. 
from  Hg  without  decomp.  at  any  temp,  be- 
tween these  limits.     (Kerp,  Z.  anorg.   1900, 
26.  68.) 

2H2O,  of  which  the  solubility  in  100  pts.  H2O 
was  found  to  be  as  follows: 

t° 

Pts.  NaBr 

t° 

Pts:  NaBr 

t° 

Pts.  NaBr 

—21 
—20 
—15 
—10 
—  5 
0 

71.1 

71.4 
73.1 
75.1 
77.1 
79.5 

+5 
10 
15 
20 
25 

82.0 

84.5 
87.3 
90.3 
93.8 

30 
35 
40 
45 
50 

97.3 
101.3 
105.8 
110.6 
116.0 

Sodium  amide,  NaNH2. 

Decomp.  by  H2O  and  alcohol. 

Sodium  amidochloride,  Na2NH2Cl. 

Sol.  in  H2O  with  decomp.  fJoannis,  C.  R. 
112.  392.) 

Sodium  arsenide,  Na3As. 

Decomp.  H2O.  (Lebeau,  C.  R.  1900,  130. 
504.) 

Sodium  arsenide  ammonia,  Na3As,  NH3. 

Easily  sol.  in  liquid  NH3.  (Lebeau,  C.  R. 
1900,  130.  502.) 

SI.  sol.  in  liquid  NH3.  (Hugot,  C.  R.  1898, 
127.  554.) 

Sodium  azoimide,  NaN3. 

Not  hygroscopic.  Sol.  in  H2O.  Insol.  in 
alcohol  and  ether.  (Curtius,  B.  24.  3344.) 

40.16  pts.  are  sol.  in  100  pts.  H2O  at  10°. 

40.7       "     "     "     "  100    "    H2O    "  ]5.2. 

41.7       "     "     ""    "  100    "    H2O    "  17.0°. 

0.3153  pt.  is  sol.  in  100  pts.  abs.  alcohol  at 
16°. 

Insol.  in  pure  ether.  (Curtius,  J.  pr.  1898, 
(2)  58.  279. 

Sodium  bromide,  NaBr,  and  +2H2O. 

Not  deliquescent.  Solubility  in  H2O  dif- 
fers according  as  NaBr  or  NaBr+2H2O  is 
used.  The  following  data  for  anhydrous 


(Coppet,  A.  ch.  (5)  30.  420.) 

If  solubility  S  =  pts.  NaBr  in  100  pts.  solu- 
tion, S=40.0+0.1746tfrom  -20°  to  +40°; 
S  =  52.3+0.0125t  from  50°  to  150°.  (Etard, 
C.  R.  98.  1432.) 

100  pts.  H2O  dissolve:  at  0°,  77.5  pts.  NaBr; 
at  20°,  88.4  pts.;  at  40°,  104.2  pts.;  at  60°, 
111.1  pts.;  at  80°,  112.4  pts.;  at  100°,  114.9 
pts.  (Kremers.) 

Sat.  solution  boils  at  121°.  (Kremers,  Pogg. 
97.  14.) 

Sat.  NaBr+Aq  contains  at: 
—22°         —10°         +140°         163° 
40.1  42.5  56.5  57.5%  NaBr, 

180°       180°       210°       212°       230° 
59.5        59.0       60.9       61.0       62.0%  NaBr. 
(Etard,  A.  ch.  1894,  (7)  2.  539.) 

100  g.  sat.  NaBr+Aq  at  16.4°  contain  47 
g.  NaBr.  (Greenish,  Pharm.  J.  1900,  66. 190.) 

Solubility  of  NaBr+2H2O  in  H2O  at  30°  = 
65.5%  anhydrous  NaBr.  (Cocheret,  Dissert. 
1911.) 

Sp.  gr.  of  NaBr+Aq  at  19.5°  containing: 

5  10  15  20  25  %  NaBr, 

1.040  1.080  1.125  1.174  1.226 

30          35          40          45 
1.281     1.334     1.410     1.483     1.565 
(Gerlach,  Z.  anal.  8.  285.) 


NaBr  were  found. 
Pts.  NaBr  dissolved  by  100  pts.  H2O  at  t°. 

NaBr+Aq  containing   17.15%   NaBr  has 
sp.  gr.  20720°  =  1.1473. 
NaBr+Aq  containing  22.72%  NaBr  has 
sp.gr.  20720°  =  1.2060. 
(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  278.) 

Sp.  gr.  of  NaBr+Aq  at  20.5°. 

t° 

Pts. 
NaBr 

t° 

Pts. 
NaBr 

t° 

Pts. 
NaBr 

44.1 
51.5 
55.1 
60.3 
64.5 

115.6 
116.2 

116.8 
117.0 
117.3 

74.5 
80.5 
86.0 
90.5 

118.4 
118.6 
118.8 
119.7 

97.2 
100.3 
110.6 
114.3 

119.9 
120.6 
122.7 
124.0 

Normality  of 
NaBr+Aq 

g.  NaBr  in  100 

g.  of  solution 

Sp.  gr.  20.5°/4° 

4.33 
3.00 

1.99 
0.98 

33.57 
25.10 
17.77 
9.41 

1.3284 
1.2284 
1  .  1526 
1.0750 

Solubility  is 
of  the  formula 
Below  50°  tf 

represe 
S     110 

'nted  by  a  straight  line 
.34+0.10751. 
isually  crystallizes  with 

le  salt  i 

(Oppenheimer,  Z.  phys.  Ch.  1898,  27.  452.) 

SODIUM  BROMIDE 


837 


Sp.    gr.    at  20°   of   NaBr+Aq   containing 

Solubility  in  ethyl  alcohol  at  30°. 

M  g.  mols.  NaBr  per  liter. 

M             0.01           0.025        0.05          0.075 
Sp.  gr.  1.000732  1.002177  1.004074  1.005972 

wt.  % 

Solid  phase 

Alcohol 

NaBr 

M             0.10          0.25          6.50          0.75 

0 

59.4 

NaBr,2H2O 

Sp.  gr.  1.00788     1.01964     1.03908     1.05811 

11.79 

42.90 

31.78 

32.12 

M              1.0            1.5            2.0 
Sp.  gr.  1.07632     1.11963     1.15240 

43.22 
54.59 
65.51 

26.79 
20.83 
16.08 

(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38.  728.) 

72.36 

13.41 

76.92 

12.03 

NaBr,  2H2O+NaBr 

Sol.  in  H2SO4.     (Walden,  Z.  anorg.  1902, 

87.35 

7.44 

NaBr 

29.  384.) 

1  i\f\    -~     ~       AT^TD,.     1      A  «     ^^4-       <-*4-     1C      1O°     ^/-».v\4-r»i^ 

97.08 

3.01 

46.05  pts.  NaBr;  100  pts.  NaBr+NaCl+Aq 
sat.  at.  18-19°  contain  46.59  pts.  of  the  two 
salts;  100  pts.  NaBr+Nal+Aq  sat.  at  18-19° 
contain  63.15  pts.  of  the  two  salts;  100  pts. 
NaBr+NaCl+Nal+Aq  sat.  at  18-19°  con- 
tain 63.20  pts.  of  the  three  salts,  (v.  Hauer, 
J.  pr.  98.  137.) 


Solubility  of  NaBr  in  NaOH+Aq  at  17°. 


(Ditte,  C.  R.  1897,  124.  30.) 

Easily  sol.  in  liquid  HF.  (Franklin,  Z. 
anorg.  1905,  46.  2.) 

Very  si.  sol.  in  alcohol. 

NaBr4-2H2O  is  sol.  in  1.10  pts.  H2O  at 
15°;  in  159  pts.  absolute  alcohol  at  15°;  in 
1200  pts.  absolute  ether  at  15°.  (Eder, 
Dingl.  221.  89.) 

NaBr+2H2O  is  sol.  in  2.25  pts.  60%  alco- 
hol, and  7  pts.  90%  alcohol.  NaBr  is  sol.  in 
3  pts.  60%  alcohol,  and  10  pts.  90%  alcohol. 
(Hager.) 

100  pts.  absolute  methyl  alcohol  dissolve 
17.35  pts.  at  19.5.°  (de  Bruyn,  Z.  phys.  Ch. 
10.  783.) 

100  g.  NaBr+CHgOH  contain  0.9  g.  NaBr 
at  the  critical  temp.  (Centnerszwer,  Z. 
phys.  Ch.  1910,  72.  437.) 

At  room  temp.,  1  pt.  NaBr  by  weight  is 
sol.  in: 

4.6  pts.  methyl  alcohol  D18  0.7990. 
14.0      "  ethyl  "     D15  0.8100. 

49.7      "  propyl  D15  0.8160. 

(Rohland,  Z.  anorg.  1898,  18.  325.) 


(Cocheret,  Dissert.  1911.) 


Solubility  in  mixtures  of  methyl  and  ethyl 
alcohol  at  25°. 

P  =  %  methyl  alcohol  in  the  solvent. 
G  =  g.  NaBr  in  10  ccm.  of  the  solution. 
S  =  Sp.  gr.  of  the  sat.  solution. 


(G.  per  100  g.  H2U.) 

P 

G 

S  25°/4° 

NaOH 

NaBr 

NaOH 

NaBr 

0.00 
4.37 
10.40 
41.02 
80.69 
84.77 
91.25 
100.00 

0.293 
0.365 
0.404 
0.724 
1.251 
1.286 
1.432 
1.440 

0.8189 
0.8265 
0.8273 
0.8593 
0.9079 
0.9104 
0.9235 
0.9238 

0.0 
3.26 
9.24 
13.43 
17.17 
19.12 

91.38 
79.86 
68.85 
64.90 
63.06 
62.51 

22.35 
24.74 
28.43 
36.61 
46.96 
54.52 

59.60 

55.03 
48.00 
38.41 
29.37 

24.76 

(Herz  and  Kuhn,  Z.  anorg.  1908,  60.  155.) 


Solubility  in  mixtures  of  methyl  and  propyl 
alcohol  at  25°. 

P  =  %  propyl  alcohol  in  the  solvent. 
G  =  g.  NaBr  in  10  ccm.  of  the  solution. 
S=Sp.  gr.  of  the  sat.  solution. 


p 

G 

S  25°/4° 

0 

1.440 

0.9238 

11.11 

1.243 

0.9048 

23.8 

1.053 

0.8887 

65.2 

0.442 

0.8390 

91.8 

0.147 

0.8153 

93.75 

0.126 

0.8144 

100 

0.074 

0.8093 

(Herz  and  Kuhn,  Z.  anorg.  1908,  60.  156.) 


838 


SODIUM  STANNIC  BROMIDE 


Solubility  in  ] 
P  =  %  proDv 

nixtures  of  propyl  and  ethyl 
alcohol  at  25°. 
1  alcohol  in  the  solvent, 
in  10  ccm.  of  the  solution. 
F  the  sat  solution. 

100  pts.  H2O  at  t°  dissolve  pts.  NaCl. 

t° 

Pts.  NaCl 

Authority 

G  =  g.  NaBr 

S  =  Sp.  gr.  o 

0 

13.89 
16.90 
59.93 
109  .  73 

More  than 
at  13.89° 
35.81 
35-.  88 
37.14 
40.38 

Gay-Lussac,  A.  ch.  (2)  11. 
310. 

P 

G 

S  25°/4° 

0 
8.1 
17.85 
56.6 
88.6 
91.2 
95.2 
100 

0.293 
0.249 
0.247 
0.190 
0.111 
0.083 
0.082 
0.074 

0.8189 
0.8147 
0.8145 
0.8107 
0.8116 
0.8083 
0.8090 
0.8093 

12 
100 

35.91 
39.92 

Fehling,  A.  77.  382. 

18.75 

37.731 

Bischof. 

10-15 

35.42 

Bergmann. 

106  + 

42.86 

Griffiths,  1825. 

20 

35.9 

Schiff,  A.  109.  326. 

(Herz  and  Kuhn,  Z.  anorg.  1908,  60.  159.) 

2.05  g.  are  sol.  in  100  g.  propyl  alcohol. 
(Schlamp,  Z.  phys.  Ch.  1894,  14.  276.) 
SI.  sol.  in  acetone.    (Krug  and  M'Elroy,  J. 
Anal.  Ch.  6.  184.) 
100  g.  95%  formic  acid  dissolve  22.3  g. 
NaBr  at  18.5°.    (Aschan,  Ch.  Ztg.  1913,  37. 

Insol.  in  methyl  acetate.     (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.     (Naumann, 
B.  1910,  43.  314);  benzonitrile.     (Naumann, 
B.  1914,  47.  1370.) 
The  composition  of  the  hydrates  formed  by 
NaBr  at  different  dilutions  is  calculated  from 
determinations   of   the   lowering   of   the  fr- 
pt.  produced  by  NaBr  and  of  the  conductivity 
and  sp.  gr.  of  NaBr+Aq.     (Jones,  Am.  Ch. 
J.  1905,  34.  303.) 

All  temps.  • 

37 

Fuchs    and    Reichenbach 
1826. 

25 

35.7 

Kopp,  A.  34.  262.' 

18.75 

36.53 

C.  J.  B.  Karsten,  1840. 

1 
18.75 
100 

36.121 
36  .  724  ' 
41.076 

G.  Karsten. 

1.25 
Boiling 

36.119 
39.324 

linger,  J.  pr.  8.  285. 

18.75 
100 

35.40 
36.95 

Karsten     (?),     cited     by 
linger,  I.e. 

15.56 
100 

34.2-35.42 
36.16 

lire's  Diet. 

15 

35.837 

Michel  and  Krafft. 

1  pt.  NaCl  is  sol.  in  2.789  pts.  H2O  at  15°  (Gerlach)  ; 
in  3  pts.  H2O  at  18.75°  (Abl)  ;  in  2.8235  pts.  H2O  at  ord. 
temp.  (Bergmann);  in  2.7647  pts.  boiling  H2O  (Berg- 

Sodium  stannic  bromide. 
See  Bromostannate,  sodium. 

Sodium  uranous  bromide,  Na2UBr6. 

As  K  salt.  (Aloy,  Bull.  Soc.  1899,  (3)  21. 
264.) 

Sodium  zinc  bromide,  NaBr,  ZnBr2+H2O. 
Hygroscopic.     (Ephraim,  Z.   anorg.   1908, 

2NaBr,  ZnBr2+5H2O.  Hygroscopic. 
(Ephraim.) 

Sodium  carbide,  Na2C2. 

Insol.  in  all  neutral  solvents;  decomp.  on 
heating  and  by  H2O.  (Matignon,  C.  R.  1897, 
125.  1034.) 

Sodium  carbonyl,  Na2C2O2. 

Decomp.  by  H2O  with  explosion.  (Joannis, 
C.  R.  116.  1518.) 

Sodium  sw&chloride,  Na4Cl2. 

Decomp.  by  H2O  into  NaCl  and  NaOH  + 
Aq.  (Kreutz,  B.  1897,  30:  403.) 

Sodium  chloride,  NaCl. 
Sol.  in  H2O. 


tClllp.      \DULglLlCiLlLlJ  ,     111     ^.(LTX*      pta.     U^lllUg     A-L'/W     V 

mann);  in  2.857  pts.  hot  or  cold  H2O  (Fourcroy). 

Not  deposited  from  boiling  aqueous  solution  unless 
the  vessel  containing  it  is  open  to  the  air.    (linger,  I.  c.) 


Solubility  in  100  pts.  H2O  at  t°. 


t° 

Pts.  NaCl 

t° 

Pts.  NaCl 

1.5 
13.75 

33.6 
35.8 

70 
108.5 

38.1 
39.4 

(Nordenskjold,  Pogg.  136.  315.) 


Solubility  in  100  pts.  H2O  at  t°. 


t 

Pts.  NaCl 

t 

Pts.  NaCl 

13.89 
16.90 

35.8 
35.9 

59  .  93 
109.73 

37.1 
40.4 

(Gay-Lussac,  A.  ch.  11.  296.) 


Solubility  of  NaCl  at  various  pressures.  The  figures 
represent  pts.  NaCl  in  100  pts.  sat.  NaCl+Aq  at 
t°  and  A  pressure  in  atmospheres. 


A 

0° 

9° 

12° 
26.35 

15° 

20° 

25° 

30° 

26.47 
26.53 

1 

20 
40 

26.25 
26.35 
26.44 

26.32 
26.38 

26.30 
26.39 
26.40 

26  .  35 
26.37 

26.37 
26.47 

(Muller,  Pogg.  117.  386.) 


SODIUM  CHLORIDE 


839 


100  pts.  H2O  -dissolve  at  t°. 

Solubility  of  NaCl  in  100  pts.  H2O  at  t°.— 
Continued. 

t° 

Pts.  NaCl 

t° 

Pts.  NaCl 

-15 
i  n 

32.73 
33.49 
34.22 
35.52 
35.63 
35.74 
35.87 
36.13 

40 
50 
60 
70 
80 
90 
100 
109.7 

36.64 
36.98 
37.25 
37.88 
38.22 
38.87 
39.61 
40.35 

t° 

90 
91 
92 
93 
94 
95 
96 

Pts. 
NaCl 

t° 

Pts. 
NaCl 

t° 

Pts. 
NaCl 

-   5 
0 
5 
9 
14 
25 

39.1 
39.1 
39.2 
39.3 
39.3 
39.4 
39.4 

97 
98 
99 
100 
101 
102 
103 

39.5 
39.6 
39.7 
39.8 
39.8 
39.9 
40.0 

104 
105 
106 
107 
108 
109 
109.7 

40.0 

40.1 
40.1 
40.2 
40.3 
40.3 
40.4 

CPoffffiale.  A.  oh.  (M  8.  649.) 

100  pts.  H2O  dissolve  at: 
0°  9°  12°  15° 

35 .59      35 . 72       35 .77       35 . 68  pts.  NaCl, 

20°        25°        30° 
35 .77    35 . 81     36 . 00  pts.  NaCl. 
(Muller,  Pogg.  122.  337.) 

100  pts.  H2O  dissolve  35.76-36.26  pts. 
NaCl  at  15.6°,  and  the  sp.  gr.  of  sat.  solution 
=  1.204.  (Page  and  Keightley,  Chem.  Soc. 
(2)  10.  566.) 

100  pts.  NaCl+Aq  sat.  at  18-19°  contain 
26.47  pts.  NaCl.  (v.  Hauer,  J.  pr.  98. 137.) 

Solubility  of  NaCl  in  100  pts.  H2O  at  t°. 


t° 

Pts. 
NaCl 

t° 

Pts. 
NaCl 

t° 

Pts. 
NaCl 

0 

35.7 

30 

36.3 

60 

37.3 

1 

35.7 

31 

36.3 

61 

37.3 

2 

35.7 

32 

36.3 

62 

37.4 

3 

35.7 

33 

36.4 

63 

37.4 

4 

35.7 

34 

36.4 

64 

37.5 

5 

35.7 

35 

36.4 

65 

37.5 

6 

35.7 

36 

36.5 

66 

37.6 

7 

35.7 

37 

36.5 

67 

37.7 

8 

35.7 

38 

36.5 

68 

37.7 

9 

35.7 

39 

36.6 

69 

37.8 

10 

35.8 

40 

36.6 

70 

37.9 

11 

35.8 

41 

36.6 

71 

37.9 

12 

35.8 

42 

36.7 

72 

38.0 

13 

35.8 

43 

36.7 

73 

38.0 

14 

35.8 

44 

36.8 

74 

38.1 

15 

35.9 

45 

36.8 

75 

38.2 

16 

35.9 

46 

36.8 

76 

38.2 

17 

35.9 

47 

36.9 

77 

38.2 

18 

35.9 

48 

36.9 

78 

38.2 

19 

36.0  • 

49 

36.9 

79 

38.3 

20 

36.0 

50 

37.0 

80 

38.4 

21 

36.0 

51 

37.0 

81 

38.4 

22 

36.0 

52 

37.0 

82 

38.5 

23 

36.1 

53 

37.1 

83 

38.6 

24 

36.1 

54 

37.1 

84 

38.6 

25 

36.1 

55 

37.1 

85 

38.7 

26 

36.1 

56 

37.2 

86 

38.7 

27 

36.2 

57 

37.2 

87 

38.8 

28 

36.2 

58 

37.2 

88 

38.9 

29 

36.2 

59 

37.3 

89 

39.0 

(Calculated  by  Mulder  from  his  own  and 
other  observations,  Scheik.  Verhandel. 
1864.  37.) 


Solubility  in  100  pts.  H2O  at: 
0-4°  20°         40°        60°         80° 

35.630    35.825    36.32    37.06    38.00 

(Andreae,  J.  pr.  (2)  29.  456.) 


Solubility  in  100  pts.  H2O  from  most  care- 
ful experiments. 


0°  20° 

35.571        35.853 

(Raupenstrauch,  M.  Ch.  6.  563.) 


60° 
37.091 


80° 
38.046 


Solubility  of  NaCl  in  100  pts.  H2O  at  t°. 


t° 

Pts.  NaCl 

t° 

Pts.  NaCl 

-14.0 

32.5 

44.75 

36.64 

-13.8 

32.15 

52.5 

37.04 

-  6.25 

34.22 

55.0 

36.99 

-  5.95 

34.15 

59.75 

37.31 

0 

35.7 

71.3 

37.96 

3.6 

35.79 

74.45 

37.96 

5.3 

35.8 

82.05 

38.41 

14.45 

35.94 

86.7 

38.47 

20.85 

35:63 

93.65 

38.90 

25.45 

35.90 

101.7 

40.76 

38.55 

36.52 

Solubility  above  20°  is  represented  by  the 
formula  S  =  34.359+0.0527t.  (Coppet,  A. 
ch.  (5)  30.  426.) 


Solubility  of  NaCl  in  100  pts.  H2O  at  high 
temp. 


t° 

Pts.  NaCl 

t° 

Pts.  NaCl 

118 
140 

39.8 
42.1 

160 
180 

43.6 
44.9 

(Tilden  and  Shenstone,  Phil.  Trans.  1884.  23.) 


840 


SODIUM  CHLORIDE 


Sat.  NaCl+Aq  contains  %  NaCl  at  t°. 

Solubility  of  NaCl  in  H2O  at  24.5°  at  vary- 
ing pressures. 

S=g,  NaCl  in  100  -g.  solvent. 
P=  pressure  in  atmospheres. 

t° 

•    %  NaCl 

t° 

%  NaCl 

-21 
-21 
-18 
17 

23.7 
23.4 
23.5 
23.3 
25.5 
25.8 
26.7 
26.8 

77 
90 
115 
135 
140 
150 
180 
215 

28.0 
28  2 
29^1 
28.9 
28.8 
29.6 
30.2 
31.6 

P 

s 

100  g.  of  solution  contains 
g.  NaCl 

-   7 
0 
+15 
55 

1 
250 
500 
1000 
1500 

35.90 
36.25 
36.55 
37.02 
37.36 

•    26.42 
26.61 
26.77 
27.02 
27.20 

100  g.  H2O  dissolve  0.616  gram-equiva- 
lent NaCl  at  25°.  (Van't  Hoff  and  Meyer- 
hoffer,  Z.  phys.  Ch.  1904,  49.  3150 


Solubility  of  NaCl  in  H2O  at  t°. 
Most  careful  experiments. 


,. 

g.  NaCl 

g.  NaCl 

t° 

per  100 

Sp.  gr. 

t° 

per  100 

Sp.  gr. 

g.  H2O 

g.  H20 

0.35 

35.75 

1.2090 

61.70 

37.28 

1.1823 

15.20 

35.84 

1.2020 

75.65 

37.82 

1.1764 

30.05 

36.20 

1.1956 

90.50 

38.53 

1.1701 

45.40 

36.60 

1.1891 

107 

39.65 

1.1631 

(Berkeley,  Phil.  Trans.  Roy.  Soc.  1904,  203. 
A.  189.) 


Sat.  NaCl+Aq.  at  25°  contains  26.5% 
NaCl.  (Foote,  Am.  Ch.  J.  1906,  36.  239.) 

100  g.  H2O  dissolve  35.80  g.  NaCl  at  25°. 
(Cameron,  Bell  and  Robinson,  J.  phys.  Ch. 
1907,  11.  396.) 

100   g.    NaCl+Aq.    sat.    at    15°   contains 

26.3  g.  NaCl;  at  30°,  26.47  g.     (Schreine- 
makers,  Arch.  nee>.  Sc.  1910,  (2)  15.  81.) 

5.456  g.  mol.  are  contained  in  1  1.  NaCl  + 
Aq  sat.  at  25°.  (Herz,  Z.  anorg.  1911,  73. 
274.) 

5.40  g.  mol.  are  contained  in  1 1.  NaCl+Aq 
sat.  at  30°.  (Masson,  Chem.  Soc.  1911,  99. 
1136.) 

26.47  g.  NaCl  are  contained  in  100  g. 
NaCl+Aq.  sat.  at  30°.  (Cocheret,  Dissert. 
1911.) 

35.79  g.  NaCl  are  sol.  in  100  g.  H2O  at 
room  temp.  (Frankforter,  J.  Am.  Chem. 
Soc.  1914,  36.  1106.) 

100  mol.  H2O  dissolve  at: 
19.3°       29.7°       40.1°       54.5° 

11.04  11.06       11.15       11. 35  mol.  NaCl. 

(Sudhaus,  Miner.  Jahrb.  Beil.  Bd.  1914,  37. 

18.) 


(Cohen,   Inouye  and  Euwen,  Z.  phys.  Ch. 
1910,  75.  257.) 


Sp.  gr.  of  NaCl+Aq  containing  15%  NaCl  is  1.109  at 
15°  (Francoeur);  1.116  at  15°  (Soubeiran);  1.1107  at  15° 
(Coulier);  1.111  at  15°  (Baudin,  C.  R.  68.  932). 

Sp.  gr.  of  NaCl+Aq  saturated  at  15°  is  1.20715 
(Michel  and  Krafft) ;  at  17.5°  is  1.2046  (Karsten) ;  at  8° 
is  1.205  (Anthon). 


.  gr.  of  NaCl+Aq. 


%  NaCl    Sp.  gr.      %  NaCl    Sp.  gr.      %  NaCl  Sp.  gr. 

5  1.037  15  1.112          25  1.192 

10  1.074  20  1.154          26.43      1.204 


(Dahlmann,  J.  B.  7.  321.) 


Sp.  gr.  of  NaCl+Aq  at  20°.      , 


%  NaCl 

Sp.  gr. 

%  NaCl 

Sp.  gr. 

1 

1.0066 

15 

1.1090 

2 

1.0133 

16 

1.1168 

3 

1.0201 

17 

1  .  1247 

4 

1.0270 

18 

1.1327 

5 

1.0340 

19 

1.1408 

6 

1.0411 

20 

1  .  1490 

7 

1.0483 

21 

1.1572 

8 

1.0556 

22 

1.1655 

9 

1.0630 

23 

1.1738 

10 

1.0705 

24 

1.1822 

11 

1.0781 

25 

1.1906 

12 

1.0857 

26 

1.1990 

13 

1.0934 

27 

1.2075 

14 

1.1012 

t 

(Schiff,  A.  110.  76.) 


Sp.  gr.  of  NaCl+Aq  at  19.5°. 


%  NaCl 

Sp.  gr. 

%  NaCl 

Sp.  gr. 

6.402 
12.265 
17.533 

1.0460 
1.0895 
1.1303 

22.631 
26.530 

1.1712 
1.2036 

(Kremers,  Pogg.  95.  120.) 


SODIUM  CHLORIDE 


841 


Sp.  gr.  of  NaCl+Aq  at  15°. 

Sp.  gr.  of  NaCl+Aq  at  20°.    x  =  mols.  NaCl 
to  100  mols.  H2O. 

%  NaCl 

Sp.  gr. 

%  NaCl 

Sp.gr. 

x                    Sp  gr.                     x 

Sp.  gr. 

1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 

.00725 
.01450 
.02174 
.02899 
.03624 
.04366 
1.05108 
1.05851 
1.06593 
1.07335 
1.08097 
1.08859 
1.09622 
1  .  10384 

15 

16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
26.395 

1.11146 
1.11938 
1  .  12730 
1  .  13523 
1.14315 
1.15107 
1.15931 
1  .  16755 
1  .  17580 
1  .  18404 
1  .  19228 
1.20098 
1.20433 

0.5           1.01145           4.0           1.08408 
1.0           1.02255           5.0           1.10276 
2.0           1.01393 

(Nicol,  Phil.  Mag.  (5)  16.  122.) 

Sp.  gr.  of  NaCl+Aq  at  0°.    S  =  weight  of  salt 
in  100  g.  of  solution  of  the  given  sp.  gr.; 
Si  =  No.  mols.  of  salt  contained  in  100 
mols.  of  the  solution. 

S 

Si 

Sp.  gr. 

(Gerlach,  Z.  anal.  8.  279.) 
Sp.  gr.  of  NaCl+Aq  at  18°. 

23.0821 
19.1932 
14.3415 
9.4120 
5.1536 

8.627 
6.769 
4.898 
3.097 
1.644 

1.1821 

1  .  1502 
1.1111 
1.0722 
1.0394 

(Charpy,  A.  ch.  (6)  29.  23.) 
Sp.  gr.  of  NaCl+Aq. 

%  NaCl 

Sp.  gr. 

%  NaCl 

Sp.  gr. 

5 
10 
15 
20 

1.0345 
1.0707 
1  .  1087 
1  .  1477 

25 

26 
26.4 

1.1898 
1  .  1982 
1.2014 

G.  -equivalents 
NaCl  per  liter 

t° 

Sp.  gr.  t°/t° 

(Kohlrausch,  W.  Ann.  1879.  1.) 

Sp.    gr.    of    NaCl+Aq    at    20°,    containing 
n  mols.  H2O  to  1  mol.  NaCl. 

0.005028 
0.01005 
0.02005 
0.04983 
0.09873 
0.19388 
0.28999 
0.47574 

18.549 
18.550 
18.538 
18.509 
18.525 
18.542 
18.559 
18.558 

1.0002119 
1.0004258 
.000848 
.002101 
.004143 
.008093 
.012053 
.019627 

n 

Sp.  gr. 

n 

Sp.  gr. 

12.5 
25 
50 

1.15292 
'  1.08207 
1.04227 

100 
200 

1.02069 
1.00965 

0.49860 
4.9860 

18.06 
17.85 

1.02054 
1.18783 

0.00259 
0.005178 
0.010318 
0.12580 
0.25019 

14.07 
14.076 
14.097 
14.097 
14.076 

1.0001108 
1.0002210 
1.0004401 
1.005315 
1.010505 

(Marignac,  J.  B.  1870.  110.) 

Sp.  gr.  of  NaCl+Aq  at  0°.    NaCl  =  g.  NaCl 
to  100  g.  H2O;  d°=sp.  gr.  at  0°;  dT  = 
maximum  sp.  g>  .;  T  =temp.  of  maximum. 

(Kohlrausch,  W.  Ann.  1894,  53.  26.) 
Sp.  gr.  of  NaCl+Aq  at  18°/18°. 

G.  NaCl                 d° 

dT 

T 

0             1.00000 
0.5          1.003925 
1              1.007634 
2              1.015366 
3              1.023530 
4              1.030669 
6             1.045975 

1.000130 
1.003988 
1.007666 
1.015367 
1.023583 
1.030890 
1.046952 

+  4° 
+  3 
+  1.77 
—  0.58 
—  3.24 
—  5.63 
—11.07 

g.  -equivalents  of  NaCl 
in  1  liter  of  solution 

Sp.  gr. 

0.005                         1.0002104 
0.010                         1.0004206 
0.020                         1.0008476 
0.050                         1.002109 
0.100                         1.004205 

(Rosetti,  A.  ch.  (4)  17.  382.) 

(Tammann,  Z.  phys.  Ch.  1895,  16.   93.) 

842 


SODIUM  CHLORIDE 


Sp.  gr.  of  NaCl+Aq  sat.  18.0°,  when 
cent  strength  of  solution;  d  =  ( 
density;  and  w= volume  cone,  in  grams 

'pd 
per  cc.  ' 


P 

d 

25.37 

.1928 

21.25 

.1592 

17.35 

.1277 

13.25 

.0958 

9.34 

.0665 

4.810 

1.0332 

2.991 

1.0202 

2.593 

1.0173 

1.746 

1.0111 

0.30263 

0.24637 

0.19503 

0.14518 

0.09960 

0.04969 

0.03052 

0.2638 

0.01765 


(Barnes.  J.  Phys.  Chem.  1898,  2.  544.) 


Sp.  gr.  of  NaCl+Aq  at  20.5°. 


Normality  of 
NaCl  +Aq 

G.  NaCl  in 
100  g.  of 
solution 

Sp.  gr.  20.5°/4° 

3.97 
2.96 
2.01 
0.97 

20.22 
15.56 
10.90 
5.49 

1.1489 
1.1124 
1.0775 
1.0373 

(Oppenheimer.  Z.  phys.  Ch.  1898,  27.  451.) 


Sp.  gr.  of  NaCl+Aq  at  15°. 


Per  cent  NaCl 

Sp.  gr. 

0 
5 
10 
15 

20 
25 
Sat.  at  15° 

1.00000 
1.03624 
1.07335 
1.11146 
1  .  15107 
1  .  19228 
1.20433 

(H.  C.  Hahn,  J.  Am.  Chem.  Soc.  1898,  20. 
622.) 


Sp.  gr.  of  NaCl+Aq  at  18°/4°. 


g.  NaCl  in  100  g.  of 
solution 

Sp.  gr. 

0.19560 
0.097952 
0.065410 
0.048977 

1.0001 
0.9994 
0.99918 
0.99905 

(Jahn,  Z.  phys.  Ch.  1900,  33.  572.) 

Sp.  gr.  20°/4°  of  a  normal  solution  of  NaCl 
=  1.03866.  (Haigh,  J.  Am.  Chem  Soc 
1912,  34.  1151.) 


Sp.  gr.  of  sat.  NaCl+Aq  at  t°. 


t° 

g.  NaCl  sol.  in 
100  g.  H2O 

Sp.  gr. 

—10° 

32.90 

1.200 

0 

35.63 

1.210 

10 

35.69 

1.205 

20 

35.82 

1.202 

30 

36.03 

1.198 

40 

36.32 

1.193 

50 

36.67 

1.189 

60 

37.06 

1.184 

70 

37.51 

1.178 

(Tschernaj,  J.  Russ.  Phys.  Chem.  Soc.  1912, 
44.  1565.) 

Sp.  gr.  of  dil.  NaCl+Aq  at  20.004°. 
Cone.  =g.  equiv.  NaCl  per  1.  at  20.004°. 
Sp.  gr.  compared  with  H2O  at  20. 004°  =  1. 


Cone. 

Sp.  gr. 

0.0000 
0.0001 
0.0002 
0.0005 
0.0010 
0.0020 
0.0040 
0.0050 
0.0100 

1.000,000,0 
1.000,004,2 
1.000,008,5 
1.000,021,3 
1.000,042,7 
1.000,085,1 
1.000,169,6 
1.000,211,7 
1.000,423,3 

(Lamb  and  Lee,  J.  Am.  Chem.  Soc.  1913,  35. 
1686.) 

The  saturated  solution  boils  at  109°. 
(Kremers.) 

NaCl+Aq  containing  42.9  pts.  NaCl  to  100 
pts.  H2O  boils  at  106.8°  (Griffiths);  contain- 
ing 41.2  pts.  NaCl  to  100  pts.  H2O  boils  at 
108.2°  (Legrand);  containing  40.38  pts. 
NaCl  to  100  pts.  H2O  boils  at  109.73°  (Gay- 
Lussac);  containing  38.7  pts.  NaCl  to  100  pts. 
H2O  forms  a  crust  at  108.3°;  highest  point  ob- 
served, 108.8°  (Gerlach,  Z.  anal.  26.  426.) 

Boiling-point  of  NaCl-f-Aq. 


%  NaCl 

B.-pt.  according  to 

Bischof 

G.  Karsten 

5 
10 
15 
20 
25 
29.4 

101.50° 

103.03 
104.63 
106.26 
107.93 
107.9-108.99 

101  .  10° 
102.38 
103.83 
105.46 
107.27 

%  NaCl 

B.-pt.  according  to 

Legrand 

Gerlach 

5 
10 
15 
20 
25 

100.80° 
101.75 
103.00 
104.60 
106.60 

100.9° 

101.9 
103.3 
105.3 
107.6 

SODIUM  CHLORIDE 


843 


B.-pt.  of  NaCl+Aq  containing  pts.  NaCl  to 
100  pts.  H2O.    G  =  according  to  Gerlach 
(Z.  anal.  26.  438;  L  =  according  to  Le- 
grand  (A.  ch.  (2)  69.  431). 

Solubility  in  HCl+Aq  at  10-10.5°. 

g.  per 

100  cc. 

G.  per  100  cc. 

HC1 

NaCl 

HC1 

NaCl 

B.-pt. 

G 

L 

B.-pt. 

G 

L 

0.0 

9.84 
12.76 
15.68 
20.78 

35.77 
33.76 
33.19 
32.71 
31.77 

26.06 
94.77 
102.1 
120.6 

30.89 
20.01 
19.04 
16.03 

100.5° 
101 
101.5 
102 
102.5 
103 
103.5 
104 
104.5 
105 

3.4 
6.6 
9.6 
12.4 
14.9 
17.2 
19.4 
21.5 
23.5 
25.5 

4.4 
7.7 
10.8 
13.4 
15.9 
18.3 
20.7 
23.1 
25.5 
27.7 

105.5° 
106 
106.5 
107 
107.5 
108 
108.4 
108.5 
108.8 

27.5 
29.5 
31.5 
33.5 
35.5 
37.5 

39^5 
40.7 

29.8 
31.8 
33.9 
35.8 
37.7 
39.7 
41.2 

(Enklaar,  R.  t.  c.  1901,  20.  183.) 
Solubility  in  HCl+Aq  at  30°. 

Composition  of  the  solution 

B.-pt.  of  NaCl+Aq  containing  g.  NaCl  in 
100  g.  H20. 
g.  NaCl        7.6      11.0      14.9      16.1      18.8 
B.-pt.        102.2°    103      104.2    104.8    106.1 

g.  NaCl      22.3       24.0    26.0     28.7 
B.-pt.        107.1      107.7108.7    109.5 
(Richmond,  Analyst,  1893,  18.  142.) 

%  by  wt.  HC1 

%  by  wt.  NaCl 

0 
6 
12 
17 
35 

.93 
.50 
.35 
.60 

26. 
16. 
9. 
4. 
0. 

47 
16 
35 
52 
11 

(Schreinemakers,  Z.  phys.  Ch.  1909,  68.  85.) 

If  NaCl  is  dissolved  in  15  pts.  H2O, .  heat 
is  absorbed  if  the  temp,  is  15°,  but  much  less 
if  temp,  is  86°;  at  100°  there  is  neither  ab- 
sorption nor  evolution  of  heat.  (Berthelofc, 
C.  R.  78.  1722.) 

36  pts.  NaCl  mixed  with  100  pts.  H2O  at 
12.6°  lower  the  temp.  2.5°.  (Riidorff,  B.  2. 
68.) 

33  pts.  NaCl  with  100  pts.  snow  at  — 1° 
give  a  temp,  of  — 21.3°.  (Riidorff,  Pogg.  122. 
337.) 

The  freezing-point  of  NaCl+Aq  is  lowered 
0.60°  for  every  gram  ftaCl  up  to  10  g. 
When  more  cone,  the  freezing-point  sinks  pro- 
portional to  NaCl,  2H2O,  0.342°  for  every 
gram  of  that  salt.  (Riidorff,  Pogg.  113. 
163.) 

Insol.  in  cone.  HCl+Aq. 

Solubility  of  NaCl  in  HC1  +  Aq  at  0°.  NaCl  = 
mols.  NaCl  (in  milligrams)  dissolved 
in  10  ccm.  of  liquid;  HCl  =  mols.  HCl  (in 
milligrams)  dissolved  in  10  ccm.  of  liquid. 


NaCl 

HCl 

Sum  of  mols. 

Sp.  gr. 

53.5 

1 

54.5 

.2045 

52.2 

1.85 

54.05 

.2025 

48.5 

5.1 

53.6 

.196 

44.0 

9.275 

53.275 

.185 

37.95 

15.05 

53.00 

.1725 

23.5 

30.75 

54.95 

.141 

6.1 

56.35 

62.45 

1.1159 

(Engel,  Bull.  Soc.  (2)  46.  654.) 


Solubility  in  HCl+Aq. 

Cone.  =  concentration    of    HCl.    g.     mol. 
per  1,000  g.  H2O. 

NaCl  =  wt.  NaCl  dissolved  in  1,000  g.  H2O. 


t° 

Cone. 

NaCl 

Molecular 
solubility 

0 

0 
0.25 
0.50 
l.CO 

357.75 
341.70 
324.45 
291.20 

6.13 
5.85 
5.56 
4.99 

25 

0 
0.25 
0.50 
1.00 

360.80 
344.50 
329.05 
298.10 

6.18 
5.90 
5.64 
5.10 

(Armstrong  and  Eyre,   Proc.  R.  Soc.   1910, 
(A)  84.  127.) 


Solubility  in  HCl+Aq  at  30°. 


(Jr.  mols.  per  1. 

HCl 

NaCl 

Sp.  gr. 
30° 

HCl 

NaCl 

Sp.  gr. 
30° 

0.0 
0.4575 
0.969 
1.786 
2.412 

5.400 
4.932 
4.386 
3.589 
2.412 

1.2018 
1  .  1906 
1.1801 
1.1633 
1.1512 

3.052 
4.152 
5.950 
7.205 

2.463 
1.628 
0.630 
0.268 

1.1427 
1.1289 
1.1188 
1.1258 

(Masson,  Chem.  Soc.  1911,  99.  1132.) 

844 


SODIUM  CHLORIDE 


Solubility  in  HCl-f-Aq  at  25°. 

Solubility  in  NaOH+Aq  at  0°.    NaCl  =  mols. 
NaCl  (in  milligrams)  in  10  ccm.  solution; 
Na2O=mols.    Na2O    (in  milligrams)    in 
10  ccm.  solution. 

Millimols  HC1  in 

10  ccm. 

Millimols  NaCl  in  10  ccm. 

e'o7 

10.32 
15.90 
21.17 
32.83 

54.56 

48.50 
44.67 
37.82 
32.97 
23.43 

NaCl 

Na20 

Na20  + 
NaCl 

Sp.  gr. 

54.7 
49.375 
47.212 
42.375 
39.55 
24.95 
19.3 
9.408 

0 
4.8 
6.725 
10.406 
14.78 
30.5 
37.875 
53.25 

54.7 
54.175 
53.937 
52.781 
54.33 
55.45 
57.175 
62.66 

1.207 
1.221 
1.225 
1.236 
1.249 
1.295 
1.314 
1.362 

(Herz,  Z.  anorg.  1912,  73.^274.) 

Moderately  dil.  H2SO4  or  HNO3+Aq  pre- 
cipitate NaCl  from  NaCl-f-Aq.     (Karsten.) 
Sol.  in  H2SO4.     (Walden,  Z.  anorg.  1902, 
29.  384.) 

Solubility  of  NaCl  in  NH4OH+Aq  at  30°. 
(G.  in  1  1.  sat.  solution.) 

(Engel,  C.  R.  112.  1130.) 

Solubility  in  NaOH+Aq  at  20°. 

G.  NaOH  in 
1  liter 

G.  NaCl  in 
1  liter 

Sp.  gr. 

deg.  Baume 

10 
20 
30 
40 
50 
60 
70 
80 
90 
100 
110 
120 
130 
140 
150 
160 
170 
180 
190 
200 
210 
220 
230 
240 
250 
260 
270 
280 
290 
300 
310 
320 
330 
340 
350 
360 
370 
380 
390 
400 
410 
420 
430 

308 
308 
306 
302 
297 
286 
277 
269 
261 
253 
244 
236 
229 
221 
213 
205 
197 
189 
181 
173 
165 
159 
152 
146 
139 
134 
129 
124 
118 
112 
107 
101 
96 
90 
85 
80 
76 
71 
66 
61 
56 
52 
48 

1.200 
1.210 
1.215 
1.225 
1.230 
1.235 
1.240 
1.245 
1.250 
1.250 
1.252 
1.252 
1.260 
1.265 
1.270 
1.275 
1.275 
1.280 
1.285 
1.290 
1.295 
1.295 
1.300 
1.303 
1.305 
1.310 
1.315 
1.320 
1.325 
1.330 
1.333 
1.335 
1.340 
1.345 
1.350 
1.355 
1.360 
1.365 
1.370 
1.375 
1.380 
1.385 
1.390 

23.5 
24.0 
25.5 
26.4 
26.9 
27.4 
27.9 
28.4 
28.8 
28.8 
29.0 
29.0 
29.7 
30.2 
30.6 
31.1 
31.1 
31.5 
32.0 
32.4 
32.8 
32.8 
33.3 
33.5 
33.7 
34.2 
34.6 
35.0 
35.4 
35.8 
36.0 
36.2 
36.6 
37.0 
37.4 
37.8 
38.2 
38.6 
39.0 
39.4 
40.0 
40.2 
40.6 

Sp.  gr. 

NH3 

NaCl 

ISp.  gr.        NH3 

NaCl 

1.17352 
1  .  1656  4 
1.160    4 
1  .  1494  6 

!9.535 
-0.655 

7.26 
0.78 

293.38 
292.5 

289.7 
286.5 

1.140872.07 
1.139572.715 
1.130181.855 
1.205    97.49 

283.38 
283.06 
277.49 
270.57 

(Hempel  and   Tedesco,  Z.  anorg.   1911,  24. 
2467.) 

Solubility  of  NaCl  in  NH4Cl+Aq  at  t°. 

t° 

G.  per  100  g.  H2O 

Sp.  gr. 

NH4C1 

NaCl 

0 

0 
146. 

1 

356.3 

286.4 

M85 

15 

0 
57. 

118. 
186. 
198. 

3 
9 

4 

8 

357.6 
326.4 
300 
271.6 

266.8 

1 
1 
1 

1 
1 

!200 
.191 
.183 
.176 
.175 

30 

0 
255. 

4 

360.3 
249 

1*168 

45 

0 
322. 

1 

365 
233.9 

.   .  . 

(Fedotieff,  Z.  phys.  Ch.  1904,  49. 
See  also  under  NH4C1. 

168.) 

SODIUM  CHLORIDE 


845 


Solubility  in  NaOH+Aq  at  20°.— Continued. 


G.  NaOH  in 
1  liter 

G.  NaCl  in 
1  liter 

Sp.  gr. 

deg.  Baum6 

440 

45 

1.395 

41.0 

450 

42 

.400 

41.5 

460 

39 

.405 

41.9 

470 

37 

.410 

42.0 

480 

34 

.415 

42.3 

490 

32 

.420 

42.6 

500 

30 

.425 

43.0 

510 

28 

.430 

43.5 

520 

27 

1.435 

43.7 

530 

27 

1.440 

44.0 

540 

26 

1.445 

44.3 

550 

26 

1.450 

44.6 

560 

25 

1.450 

44.6 

570 

24 

1.455 

45.0 

580 

23 

1.460 

45.5 

590 

23 

1.465 

45.9 

600 

22 

1.470 

46.2 

610 

21 

1.475 

46.5 

620 

20 

1.480 

46.8 

630 

19 

1.485 

47.0 

640 

18 

1.490 

47.5 

(Winteler,  Z.  Elektrochem,  1900,  7.  360.) 
Solubility  in  Na2O+Aq  at  30°. 


Composition 

of  the  solution 

%  by  wt. 
Na'O 

%  by  wt. 
NaCl 

Solid  phase 

0 

26.47 

NaCl 

4.47 

21.49 

t 

12.22 

13.62 

i 

24.48 

4.36 

f 

29.31 

2.40 

i 

37.85 

1.12 

1 

41.42 

0.97 

NaCl+NaOH,  H2O 

42 

0 

NaOH,  H2O 

(Schreinemakers,  Z.  phys.  Ch.  1909,  68.  85.) 

The  presence  of  other  salts  increases  the 
solubility  of  NaCl  in  H2O. 

Sol.  in  sat.  NH4Cl+Aq  with  pptn.  of 
NH4C1.  When  the  reaction  is  complete, 
the  solution  has  sp.  gr.  1.1788,  and  contains 
32.62%  mixed  salts;  or  100  pts.  H2O  dissolve 
48.42  pts.  mixed  salts,  viz.,  26.36  pts.  NaCl 
and  22.08  pts.  NH4C1.  (Karsten.)  (See 
under  NH4C1.) 

Sol.  in  sat.  BaCl2+Aq  with  pptn.  of  BaCl2 
until  a  state  of  equilibrium  is  reached,  when 
100  pts.  H2O  at  17°  dissolve  38.6  pts.  of  mixed 
salts,  of  which  4.1  pts.  are  BaCl2.  (Karsten.) 
(See  under  BaCl2.) 

Insol.  in  sat.  CaCl2+Aq.  (Vauquelin, 
Ann.  de  Chim.  13.  95.) 

Much  more  sol.  in  hot  than  in  cold  H2O 
containing  MgCl2  or  CaCl2;  but  NaCl  is  pptd. 
from  sat.  NaCl+Aq  when  that  solution  is 
mixed  with  MgCl2  or  CaCl2  +  Aq.  (Fuchs  and 
G.  Reichenbach,  1826.)  (See  under  MgCl2.) 


Less  sol.  in  cone.  CaCl2+Aq  than  in  H2O. 
(Hermann.) 

Solubility  of  NaCl+CaCl2  in  H2O  at  25°. 
G.  per  100  g.  H2O. 


NaCl 


0 

1.846 
1.637 
1.799 
7.77 
10.70 
18.85 
32.48 
35.80 


CaCh 


84 

78.49 

58.48 

53.47 

36.80 

30.08 

19.53 

3.92 

0 


Sp.  gr. 
25°/25° 


4441 
3651 
3463 
2831 
2653 
2367 
2080 


1.2030 


Solid  phase 


CaCl2,  6H2O 
"      +NaCl 
NaCl 


(Cameron,  Bell  and  Robinson,  J.  phys.  Chem. 
1907,  11.  396.) 

Solubility   of   NaCl   in   NaHCO3   sat.   with 
CO2  at  t°. 


0 

u 

15 

^( ... 

30 
45 


G.  per  1000  g.  H2O 


NaHC03 


6.0 

7.7 
0.0 

10.0 
0.0 

13.9 
0.0 
0.23 


NaCl 


356.3 
350.1 
357.6 
354.6 
360.3 
358.1 
356.0 
361.5 


(Fedotieff,  Z.  phys.    Ch.ll904,  49.  170.) 

Sol.  in  sat.  KClO3+Aq;  the  solution  can 
then  dissolve  more  KC1O3.  (Margueritte. 
C.  R.  38.  305.) 

In  solution  containing  Na,  K,  Cl  and  NO3 
ions,  the  solubility — relations  between  the 
four  salts  NaCl,  KC1,  NaNO3  and  KNO3 
have  been  studied.  (Uyeda,  Z.  anorg.  1911, 
71.  2.) 

Sol.  in  sat.  NH4NO3+Aq,  without  causing 
pptn.  (Karsten.) 

Sol.  in  sat.  NH4NO3+Aq,  from  which  solu- 
tion it  is  not  pptd.  by  salts  which  would  cause 
its  pptn.  in  aqueous  solution.  (Margueritte, 
C.  R.  38.  307.) 

Sol.  in  sat.  Ba(NO3)2+Aq  without  causing 
pptn. 

Insol.  in  Ca(NO3)2+Aq. 

Sol.  in  Mg(NO3)2+Aq  with  pptn.  of  small 
portion  of  Mg(NO3)2. 

Sol.  in  sat.  KNO3+Aq,  the  mixed  solution 
having  the  power  to  dissolve  more  KNO3,  and 
the  solubility  of  the  KNO3  apparently  in- 
creasing in  the  same  ratio  as  the  amount  of 
NaCl  present.  (Fourcroy  and  Vauquelin, 
Ann.  de  Chim.  11.  130.) 

Sol.  in  sat.  KNO3+Aq;  the  solution  thus 


846 


SODIUM  CHLORIDE 


obtained  at  18.13°  contains  40.34%  of  the 
mixed  salts,  or  100  pts.  H2O  dissolve  67.72 
pts.  of  the  mixed  salts,  viz.,  38.25  pts.  NaCl 
and  29 . 45  pts.  KNO3.  (Karsten.) 

Solubility   of  NaCl  in   KNO3+Aq  at  25°. 
KNO3  =  g.  KNO3  in  100  cc.  of  solution. 
NaCl=g.  mol.  per  1. 


KNO3 

NaCl 

KN03 

NaCl 

0 
4 

8 

5.44 
5.52 
5.45 

12 
16 
20 

5.28 
5.21 
5.15 

(Ritzel,  Z.  Krist.  1911,  49.  152.) 
(See  also  under  KNO3.) 

Solubility  of  NaCl  in  NaNO3+Aq  at  15.5°. 


g.  per 

100  cc.  sat.  s 

olution 

Sp.  gr. 

NaNOa 

NaCl 

H20 

.2025 

0 

31.78 

88.47 

.2305 

7.53 

27.89 

87.63 

.2580 

13.24 

26.31 

86.25 

.2810 

21.58 

23.98 

82.66 

.3090 

28.18 

22.30 

80.42 

.3345 

33.80 

20.40 

79.25 

.3465 

37.88* 

19.40* 

77.37 

.3465 

37.64* 

19.67* 

77.34 

*Solutions  sat.  with  both  salts. 
(Bodlander,  Z.  phys.  Ch.  1891,  1.  361.) 

Sol.   in   sat.    NaNO3+Aq   with   pptn.    of 
NaN03. 

Solubility  of  NaCl  in  NaNO3+Aq. 
Cone.  =  concentration  of  NaNO3  in  g.  mol. 
per  1,000  g.  H2O. 

NaCl  =  g.  NaCl  dissolved  in  1,000  g.  H2O. 


t° 

Cone. 

NaCl 

Molecular 
solubility 

0 

0 

0.25 
0.50 
1 

359.65 
355.90 
351.20 
342.15 

6.16 
6.09 
6.02 

5.86 

25 

0 
0.25 
0.50 
1 
2 

362.95 
356.65 
352.30 
343.65 
325.50 

6.20 
6.11 
6.03 

5.88 
5.58 

(Armstrong  and  Eyre,  Proc.  R.  Soc.  1910,  A. 

84.  127.) 
(See  also  under  NaNO3.) 

Sol.  in  sat.  KCl+Aq  with  elevation  of 
temp.  (Vauquelin.) 

100  g.  H2O  sat.  with  KCl  dissolve  0.494 
gram-equivalent  NaCl  at  25°.  (Fuler, 
Z.  phys.  Ch.  1904,  49.  315.) 


Solubility  in 

KCl+Aq  at  t°. 

t° 

Sat.  solution  contains 

%  NaCl 

%  KCl 

-20 

21.3 

5.7 

-10 

21.3 

6.7 

0 

21.3 

7.7 

+10 

21.3 

8.6 

20 

21.3 

9.6 

30 

21.3 

10.6 

40 

21.3 

11.5 

50 

21.3 

12.5 

60 

21.3 

13.5 

70 

21.3 

14.4 

80 

20.7 

15.8 

90 

19.9 

17.8 

100 

18.8 

19.8 

110 

17.2 

22.4 

120 

16.5 

24.1 

130 

16.4 

25.1 

140 

16.4 

26.1 

150 

16.4 

27.1 

160 

16.4 

28.0 

170 

16.4 

29.0 

180 

16.4 

30.0 

(Etard.  A.  ch. 

1894,  (7)  3.  277.) 

(See  under  KC1.) 

100  pts.  NaCl+Nal+Aq  sat 

at   18-19° 

contain 

62.33   pts.    of  the  two 

salts,      (v. 

Hauer.) 

Sol.  in  sat.  Al2(SO4)3+Aq  with  no  pptn. 

(Vauquelin.) 

Sol.  in  sat.  (NH4)2SO4+Aq  with  pptn.  of 
considerable  amt.  of  (NH4)2SO4+Aq.    (Vau- 

quelin.) 

Sol.  in 

sat.  CuSO4+Aq. 

100  pts.  H2O  dissolve  36.71  pts.  NaCl  and 

7.19  pts. 

K2SO4  at  15°,  and  solution  has  sp. 

gr.  1.24. 

(Page  and 

Keightey.) 

NaCl  is  sol.  in  K2SO4+Aq,  and  vice  versa, 

without  separation  of 

a  salt. 

100  pts.  H2O  dissolve  7.03  pts. 

K2SO4  and 

37.60  pts.  NaCl,  when  warmed 

and  cooled 

to  14°. 

(Rudorff.) 

Solubility  of  NaCl  and  K2SO4  in 

H2O  at  t°. 

100 

3ts.  H2O  contain  pts.  NaCl,  K2SO4, 

and 

KC1. 

t° 

Pts.  NaCl 

Pts.  K2S04 

Pts.  KCl 

10 

33.43 

8.10 

3.18 

20 

34.01 

8.90 

3.06 

30 

34.56 

9.56 

2.95 

40 

35.16 

10.38 

2.81 

50 

35.77 

11.07 

2.84 

60 

36.40 

11.93 

2.72 

70 

36.64 

12.82 

3.20 

80 

36.04 

12.26 

5.06 

90 

35.86 

12.42 

6.98 

100 

35.63 

12.56 

8.79 

(Precht  and  Wittgen,  B.  15. 

1666.) 

SODIUM  CHLORIDE 


847 


Sol.  in  cold  sat.  NaSO4+Aq  at  first  without 
pptn.,  afterwards  Na2SO4  separates  out. 
(Karsten.) 

Solubility  in  Na2S04+Aq  containing  7.45  g. 
Na2SO4  in  100  g.  of  the  solution. 


14.80 
17.90 
24.85 
25.60 
27.75 
32.18 
34.28 


g.  NaCl  in  100  g.  of 
the  solution 


23.30 

23.33 

23.45 

23.485 

23.525 

23.55 

23.68 


(Marie  and  Marquis,  C.  R.  1903,  136.  684.) 
See  also  under  Na2SO4. 

Sol.  in  sat.  ZnSO4+Aq  with  separation  of 
Na2SO4,  ZnSO4.  (Karsten.) 

Insol.  in  liquid  CO2.  (Buchner,  Z.  phys. 
Ch.  1906,  54.  674.) 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  829.) 

12.2  pts.  NaCl  are  sol.  in  1  pt.  hydrazine  at 
12.5-13°.  (de  Bruyn,  R.  t.  c.  1899,  18.  297.) 

100  g.  hydroxylamine  dissolve  14.7  g.  NaCl 
at  17.5°.  (de  Bruyn,  Z.  phys.  Ch.  1892,  10. 
782.) 

100  g.  95%  formic  acid  dissolve  5.8  g.  at 
19.7°.  (Aschan,  Ch.  Ztg.  1913,  37.  1117.) 

Solubility  in  alcohol. 

100  pts.  alcohol  of  0.900  sp.  gr.  dissolve  5.8  pts.  NaCl; 
of  0.872  sp.  gr.  dissolve  3.67  pts.  NaCl;  of  0.834  sp.  gr. 
dissolve  0.5  pt.  NaCl.  (Kirwan.) 

100  pts.  alcohol  containing  given  %  by  weight  of 
absolute  alcohol  dissolve  pts.  NaCl  at  25°. 


% 

alcohol 

Pts. 
NaCl 

% 
alcohol 

Pts. 
NaCl 

% 
alcohol 

Pts. 
NaCl 

0.0 
8.4 
16.7 
25.1 

35.70 
30.49 
24.84 
19.30 

33.4 
41.8 
50.2 
58.5 

16.08 
13.28 
11.28 
7.96 

66.9 
75.2 
83.6 

5.95 
3.75 
1.59 

(Kopp,  A.  40.  206.) 

100  pts.  alcohol  of  75%  by  weight  dissolve  at: 

14°  15.2°  38°          71.5° 

0.661         0.700         0.736         1.033  pts.  NaCl. 

100  pts.  alcohol  of  95.5%  by  weight  dissolve  at: 

15°          77.2° 
0.174         0.171  pts.  NaCl. 
(Wagner,  A.  64.  293.) 

100  pts.  alcohol  containing  %  alcohol  by 
weight  dissolve  pts.  NaCl  at  15°,  or  100  pts. 
solution  contain  %  NaCl. 

10  20  30  40     %  alcohol, 

28.53      22.55       17.51       13.25  pts.  NaCl, 
22.2         18.4         14.9         11.7  %  NaCl, 

50  60  80  %  alcohol, 
9.77  5.93  1.22  pts.  NaCl, 
8.9  5.6  1.2  %NaCl. 


(Schiff,  A.  118.  365.) 


Solubility  of  NaCl  in  alcohol  increases  with 
the  temperature. 

100  pts.  (by  weight)  of  alcohol  of  0.9282 
sp.  gr.  (50.5%  by  weight)  dissolve  at: 

4°         10°         13°         23°        32° 
10.9      11.1      11.43      11.9      12.3  pts.  NaCl, 


33 
12.5 


44( 
13.1 


51' 
13.8 


60° 
__._     14.1  pts.  NaCl. 

(Gerardin,  A.  ch.  (4)  5.  146.) 


Solubility  in  alcohol  at  13°. 


Sp.  gr. 

100  com.  contain  in  g. 

Alcohol 

Water 

Salt 

1.2030 

0 

88.70 

31.60 

1.1348 

11.81 

78.41 

23.26 

1.1144 

15.99 

74.64 

20.81 

1.0970 

19.39 

71.45 

18.86 

1.0698 

24.95 

65.80 

16.23 

1.0295 

32.33 

57.96 

12.66 

0.9880 

40.33 

49.34 

9.13 

0.9445 

49.28 

38.54 

5.93 

0.9075 

57.91 

29.37 

3.47 

0.8700 

63.86 

21.62 

1.52 

0.8400 

72.26 

11.24 

0.50 

(Bodlander,  Z.  phys.  Ch.  7.  317.) 


Solubility  in  ethyl  alcohol +Aq  at  30°. 


wt.  % 

g.  NaCl  per  100  g. 

wt.  % 

g.  NaCl  per  100  g. 

alcohol 

solution 

H20 

alcohol 

solution 

H2O 

0 

26.50 

36.05 

50 

9.34 

20.60 

5 

24.59 

34.29 

60 

6.36 

16.96 

10 

22.56 

32.57 

70 

3.36 

12.75 

20 

19.05 

29.40 

80 

1.56 

7.95 

30 

15.67 

26.53 

90 

0.43 

4.30 

40 

12.45 

23.70 

(Taylor,  J.  phys.  Ch.  1897,  1.  723.) 


Solubility  in  ethyl  alcohol +Aq  at  40°. 


wt.  % 
alcohol 

g.  NaCl  per  100  g. 

wt.  % 
alcohol 

g.  NaCl  +100  g. 

solution 

H20 

solution 

H2O 

0 
5 
10 
20 
30 
40 

26.68 
24.79 
22.90 
19.46 
16.02 
12.75 

36.38 
34.69 
33.00 
30.20 
27.25 
24.37 

50 
60 
70 
80 
90 

9.67 
6.65 
3.87 
1.69 
0.50 

21.42 
17.82 
13.10 
8.68 
5.10 

(Taylor,  I.  c.) 


848 


SODIUM  CHLORIDE 


Solubility  of  NaCl  in  ethyl  alcohol +Aq  a 

28°. 


C&E 


0 

3.8 

7.7 

16.1 

25.3 

35.0 


%  H20 


73.53 

71.6 

69.7 

64.6 

58.9 

52.5 


NaCl 


26.47 

24.6 

22.6 

19.3 

15.8 

12.5 


C2H6OH 


45.35 

56.2 

67.4 

78.8 
89.6 


%  H20 


45.35 

37.5 

28.9 

19.7 

10 


% 

NaCl 


9.3 
6.3 
3.7 
1.5 
0.4 


(Fontein,  Z.  phys.  Ch.  1904,  73.  212.) 

Solubility  of  NaCl  in  ethyl  alcohol +Aq  at  25° 
Cone.  =  concentration  of  alcohol  in  g.  mol 

per  1,000  g.  H2O. 

NaCl  =  g.  in  1,000  g.H2O. 


Cone. 


0 

0.25 
0.50 
1 
3 


NaCl 


359.65 
355.15 
349.65 
337.80 
301 . 60 


Molecular 
solubility 


6.16 
6.08 
5.98 
5.79 
5.16 


(Armstrong  and  Eyre,  Proc.  R.  Soc.   1910, 
(A)  84.  127.) 

100  pts.  absolute  methyl  alcohol  dissolve 
1.41  pts.  at  18.5°;  100  pts.  absolute  ethyl 
alcohol  dissolve  0.085  pt.  at  18.5°.  (de 
Bruyn,  Z.  phys.  Ch.  10.  782.) 

100  pts.  wood-spirit  of  40%  (by  weight) 
dissolve  13.0  pts.  NaCl.  (Schiff,  A.  118.  365.) 

100  g.  NaCl+CH3OH  contain  0.1  g.  NaCl 
at  the  critical  temp.  (Centnerszwer,  Z.  phys. 
Ch.  1910,  72.  437.) 

Solubility  of  NaCl  in  methyl  alcohol  -f-Aq. 
at  25°. 

Cone.  =  concentration  of  alcohol  in  g.  mol. 
per  1,000  g.  H2O. 

NaCl  =  g.  in  1,000  g.  H2O. 


t 

Cone. 

NaCl 

Molecular 
solubility 

0° 

0 
0.25 
0.50 

1 

357.75 
355.20 
353.10 
347.45 

6.13 
6.08 
6.05 
5.95 

25° 

0 
0.25 
0.50 
1 
3 

362.95 
359.40 
357.60 
353.20 
336.25 

6.20 
6.14 
6.11 
6.04 
5.75 

(Armstrong  and  Eyre,  Proc.  R.  Soc.  1910, 
(A)  84.  127.) 

Traces  dissolve  in  propyl  alcohol.  (Schlamp 
Z.  phys.  Ch.  1894,  14.  276.) 


Solubility  of  NaCl  in  propyl  alcohol +Aq. 
at  25°. 

Cone.  =  concentration  of  alcohol  in  g.  mol. 
per  1,000  g.  H2O. 

NaCl  =  g.  NaCl  in  1,000  g.  H2O. 


25 


Cone. 


0 

0.25 

0.50 


0 

0.25 

0.50 


NaCl 


357.75 
351.20 
345.55 


362.95 
355.75 
350.20 


Molecu  lar 
solubility 


6.13 
6.01 
5.91 


6.20 
6.10 
6.00 


(Armstrong  and  Eyre,  Proc.  R.  Soc.  1910,  A. 
84.  127.) 

Solubility  of  NaCl  in  propyl  alcohol +Aq  at 
23-25°. 


NaCl 


0.55 

2.23 

3.55 

3.90 

5.27 

8.04 

10.49 

12.20 


/o 
C3H7OH 


87.7 

51.57 

18.99 

14.78 

12.77 

9.49 

7.79 

6.57 


11.75 
46.20 
77.46 
81.32 
81.96 
82.47 
81.72 
81.23 


NaCl 


14.38 
15.42 
16.38 
18.08 
20.12 
22.35 
24.50 
24.90 


CsHyOH 

5.39 
5.11 
4.47 
3.83 
3.27 
2.64 
2.13 
2.3 


& 

80.23 
79.47 
79.14 
78.09 
76.61 
75.01 
75.37 
72.80 


Frankforter  and  Frary,  J.  phys.  Ch.  1913, 
17.  402.) 

100  g.  sat.  solution  of  NaCl  in  99.6%  propy 
alcohol  contain  0.04  g.  NaCl  at  25°.  (Frank- 
"orter  and  Frary.) 

Insol.  in  fusel  oil.  (Gooch,  Am.  Ch.  J.  9. 
53.) 

Solubility    of    NaCl    in    amyl    alcohol +Aq. 
Liquid  phases  conjugated  at  28°. 


Upper  layer 

Lower  layer 

NaCl 

amyl 
alcohol 

H20 

NaCl 

amyl 
alcohol 

H2O 

0.05 
it 

a 
a 

0 

95.45 
94.1 
92.9 
91.6 
90.2 

4.5 
5.9 
7.1 
8.4 
9.8 

26.36 
19 
12.7 
6.2 
0 

0.22 
0.4 
0.8 
1.5 
2.3 

73.42 
80.4 
86.5 
92.3 
97.7 

(Fontein,  Z.  phys.  Ch.  1910,  73.  226.) 

At  room  temp.  1  pt.  by  weight  is  sol.  in: 
75  pts.  methyl  alcohol  D15  0.7990. 
566    "    ethyl          "       D15  0.8100. 
3000    "    propyl        "       D15  0.8160. 
(Rohland,  Z.  anorg.  1898,  18.  325.) 

100  g.  methyl  alcohol  dissolve  1.31  g.  NaCl 
t  25°. 


SODIUM  CHLORIDE 


849 


100 

„  4-   OK° 

g.  ethyl 

alcohol 

dissolve 

0.065  g.  NaCl 

Solubility  in  acetone  -f-Aq  at  20°. 

at  Jo  . 
100  g.  propyl  alcohol  dissolve  0.012  g.  NaCl 

%  NaCl 

%H20 

%  acetone 

at  25° 
100 
NaCl 

g.  isoamyl   alcohol  dissolve  0.002  g. 
at  25°. 

25.9 
24.19 

73.06 
71.18 

1.04 
4.03 

25.06 

72.00 

2.94 

(Turner  and  Bissett, 

Chem.  Soc.  1913,  103. 

20.85 

66.78 

12.37 

1909.) 

20.17 

66.01 

13.82 

18.32 

63.16 

18.52 

Solubility  of  NaCl  in 

ethyl  +  amyl  alcohol  at 

20.44 

66.19 

13.37 

28°. 

17.89 

62.21 

19.90 

0  32 

13  92 

85.76 

Upper  layer 

Lower  layer 

o!l9 

10.82 

88.99 

0.15 

9.62 

90.23 

Na°Cl 

%  amyl 
alcohol 

%  ethyl 
alcohol 

N?C1 

%amyl 
alcohol 

%  ethyl 
alcohol 

0.12 

8.94 

90.94 

0.05 

95.45 

0 

26.35 

0.22 

0 

(Frankforter  and  Cohen,  J.  Am.  Chem.  Soc. 

0.10 

86.6 

9.5 

25.30 

0.25 

1.9 

1914,  36.  1127.) 

0.25 

75.4 

19.1 

24.02 

0.3 

9.5 

0.58 

59.9 

30.9 

22.64 

0.4 

6.9 

Solubility  in  glycol  at  14.8°  =  31.7%.     (de 

1.23 

47.0 

38.7 

21.19 

0.5 

10.3 

Coninck,  Belg.  Acad.  Bull.  1905.  275.) 

2.81 

31.6 

44.8 

19.26 

1.3 

15.2 

Sol.  in  glycerine.    (Pelouze.) 

6.56 

17.7 

41.5 

15.81 

3.69 

22.1 

Critical    solution:     amyl    alcohol,     10%; 
ethyl    alcohol,    32.5%;    NaCl,    11%;    H2O, 

Solubility  of  NaCl  in  glycerine  +Aq  at  25°. 
G  =  g.  glycerine  in  100  g.  glycerine  +Aq. 
NaCl  =  millimols  NaCl  in  100  cc.  of  the 

46.5%. 

solution. 

(1*  ontein,  Z.  phys.  Ch.  1910,  73.  244.) 

G 

NaCl 

Sp.gr. 

Ether     ppts.      NaCl     from     NaCl-f-Aq. 

0 

545.6 

1  .  1960 

CGmelin.) 
Very  si.  sol.  in  a  mixture  of  equal  pts.  of 
absolute  alcohol  and  ether.    (Berzelius.) 
500  mg.  NaCl  treated  with  above  mixture 
yielded  only  0.5  mg.  to  the  liquid.    (Lawrence 
Smith,  Am*  J.  Sci.  (2)  16.  57.) 

13.28 
25.98 
45.36 
54.23 
83.84 
100 

501.1 
448.4 
370.2 
333.9 

220.8 
167.  1 

1.2048 
1.2133 
1.2283 
1.2381 
1.2696 
1  2964 

100 

pts.  of  a  mixture  of  1  pt.  96% 

alcohol 

J-V/VJ 

and  1  pt.  98%  ether  dissolve  0.11  pt 
(Mayer,  A.  98.  205.) 

NaCl. 

(Herz  and  Knoch,  Z.  anorg.  1905,  46.  267.) 

Insol.  in  acetone.     (Krug  and  M'Elroy,  J. 
Anal.  Ch.  6.  184;  Eidmann,  C.  C.  1899,  II. 

1  A1  A    \ 

Insol.    in    benzonitrile.       (Naumann,     B. 
1914,  47.  1370.) 

1014.) 

Insol.  in  methyl  acetate.     (Naumann,  B. 

Solubility  in  acetone  +Aq  at  20°. 

1909,  42.  3790);  ethyl  acetate.     (Naumann, 
B.  1904,  37.  3602.) 

A  =  ccm.  acetone  in  100  ccm.  of  the  solvent. 

NaCl  =  millimols  NaCl  in  100  ccm.  of  the 

solution. 


Solubility  of  NaCl  in  solutions  of  HgCl2  in 
ethyl  acetate. 


A 

NaCl 

100  mo  Is.  ethyl  acetate  dissolve 

0 

537.9 

Mols.  HgCl2 

Mols.  NaCl 

Mols.  HgCh 

Mols.  NaCl 

10 

4-fi4.  fi 

20 

394.8 

40.0 

20.0 

18.0 

5,1 

,      30 

330.1 

38.1 

19.6 

16.4 

4.3 

32] 

lower  layer  308  .  5 

36.0 

19.2 

14.1 

3.8 

to  >  2  phases 

34.9 

18.5 

13.2 

2.9 

87  J 

upper  layer     7  .  7 

34.8 

18.3 

12.4 

2.3 

88 

7.3 

32.1 

13.8 

12.0' 

1.6 

89 

5.6 

28.0 

9.1 

12.2 

1.3 

90 

4.3 

22.8 

7.0 

12.9 

0.8 

100 

22.9 

7.0 

(Herz  and  Knoch,  Z.  anorg.  1904,  41.  318.) 

(Linebarger,  Am.  Ch.  J.  1894,  16.  215.) 

850 


SODIUM  STANNIC  CHLORIDE 


Solubility  of  NaCl  in  urea+Aq  at  25°. 

Sodium    stannic    chloride,    2NaCl, 

See  Chlorostannate,  sodium. 

Sodium    thallic    chloride,    3NaCl, 
12H2O. 
Very  sol.   in  H2O.      (Pratt,   Am 
1895,  (3)  49.  404.) 

SnCl4+ 

T1C13  + 
J.   Sci. 

%  urea 

%  NaCl 

%  urea 

%  NaCl 

0 
5 
9.6 
13 

31.80 
30.63 
29.05 
28.46 

18 

23 

28 

27.65 
27.24 
26.56 

(Ritzel,  Z.  Kryst.  Min.  1911,  49.  152.) 

Solubility  of  NaCl  in  urea+Aq  at  (?)°. 
g  =  g.  urea  in  100  cc.  of  solution, 
sol.  =  increase    of    solubility    of    NaCl    in 
g.  per  100  cc.  of  the  solution. 


g. 

sol. 

g. 

sol. 

5 
10 
15 
20 
25 

0.044 
0.124 
0.234 
0.372 
0.529 

30 
35 
40 
45 
50 

0.709 
0.910 
1.134 
1.370 
1.602 

(Fastert,  N.  Jahrb.  Min.  Beil.  Bd.  1912,  23. 

286.) 

Solubility  of  NaCl  in  formamide+Aq  at  25°. 

%  HCONH2 

%  NaCl 

%HCONH2 

%  NaCl 

0 
2.3 
5.3 

8 

31.80 
30.98 
30.86 
30.40 

11 

15 

18.8 

29.11 

28.52 
27.76 

(Ritzel,  Z.  Kryst.  Min.  1911,  49.  152.) 

Insol.  in  anhydrous  and  in  97%  pyridine. 
Very  si.  sol.  in  95%  pyridine+Aa.  SI.  sol. 
in  93%  pyridine+Aq.  (Kahlenberg,  J.  Am. 
Chem.  Soc.  1908,  30.  1107.) 

Insol.  in  oil  of  turpentine.  (T.  S.  Hunt, 
Am.  J.  Sci.  (2)  19.  417.) 

100  g.  H2O  dissolve  236.3  g.  sugar +42.3  g. 
NaCl  at  31.25°,  or  100  g.  sat.  aq.  solution 


(Armstrong  and  Eyre,  Proc.  R.  Soc.   1910, 
(A)  84.  127.) 

Min.  Halite. 
+2H2O.     Efflorescent  below '0°;  si.  deli- 
quescent at  temps,  above  0°.    (Fuchs,  1826.) 

The  solubility  in  H2O  at  — 12.25°  corre- 
sponds to  32.9  pts.  of  NaCl  per  100  pts.  H2O 
(Matignon,  C.  R.  1909,  148.  551.) 


Sodium  uranium  chloride,  2NaCl,  UC14. 

Non  volatile  and  not  hydroscopic.  (Mois- 
san,  C.  R.  1896,  122.  1089.) 

Sol.  in  H2O.  (Colani,  A.  ch.  1907,  (8)  12. 
59.) 

Sodium  uranyl  chloride,  Na2(UO2)Cl4. 

As  K  salt.  (Aloy,  Bull.  Soc.  1899,  (3)  21. 
264.) 

Sodium  zinc  chloride,  2NaCl,  ZnCl2+3H2O. 
Deliquescent.    Easily  sol.  in  H2O.    (Schind- 
ler,  Mag.  Pharm.  36.  48.) 

Sodium  zirconium  chloride,  2NaCl,  ZrCl4. 

(Paykull.) 
Sodium  chloroiodide,  NaCl4I+2H2O. 

Easily  decomp.  by  alcohol  or  ether.  (Wells 
and  Wheeler,  Sill.  Am.  J.  143.  42.) 

Sodium  fluoride,  NaF. 

Very  si.  sol.  in  cold,  and  not  more  abund- 
antly in  boiling  H2O.  (Rose.) 

100  pts.  H2O  dissolve  4.78  pts.  at  16°.  (Ber- 
zelius.) 

100  pts.  H2O  dissolve  4  pts.  at  15°.  (Fremy, 
A.  ch.  (3)  47.  32.) 

Sp.  gr.  of  aqueous  solutions  containing  in 
lOOpts.  H2O: 

1.1081         2.2162        3.3243  pts.  NaF. 
1.0110         1.0221         1.0333 

Sat.  solution  has  sp.  gr.  1.0486.  (Gerlach, 
Z.  anal.  27.  277.) 


(Kohler,  Z.  Ver.  Zuckerind,  1897,  47.  447.) 

Solubility  of  NaCl  in  glucose  +Aq  at  25°. 
Cone.  =  concentration  of  glucose  +Aq  in  g. 
mol.  per  1,000  g.  H2O. 
Sol.  =  Solubility  in  1,000  g.  H2O. 

taming  4.3%  NaF.     (Mylius  and  Funk,  B. 
1897,  30.  1718.) 
Solubility  of  NaF  in  HF+Aq  at  21°. 

g.  per  1000  g.  H2O 

g.  per  1000  g.  H2O 

Cone. 

Sol. 

Molecular 
solubility 

HF 

NaF 

HF 

NaF 

0.0 
10.0 

45.8 
56.5 

41.7 
41.4 
22.5 
22.7 

83.8 
129.7 
596.4 

777.4 

22.9 

23.8 
48.8 
81.7 

0 
0.25 
0.50 
1.0 

361.40 
364.15 
364.30 
369.90 

6.18 
6.22 

6.23 
6.32 

m;+f0  P.  T?    TSQfi  123.  1282.) 

Easily  sol.  in  liquid  HF.  (Franklin,  Z. 
anorg.  1905,  46.  2.) 

SI.  sol.  in  cone.  KC2H3O2+Aq.  (Strom- 
eyer.) 

Almost  insol.  in  alcohol.  (Berzelms,  Pogg 
1.  13.) 

Insol.  in  methyl  acetate.  (Naumann,  B 
1909,  42.  3790.) 


SODIUM  HYDROXIDE 


851 


Sodium  hydrogen  fluoride,  NaHF2. 

Rather  difficultly  sol.  in  cold,  more  easily 
in  hot  H2O.  (Berzelius,  Pogg.  1.  13.) 

Sodium  tantalum  fluoride. 
See  Fluotantalate,  sodium. 

Sodium  tin  (stannous)  fluoride,  2NaF,  3SnF2. 
Sol.  in  H2O.    (Wagner,  B.  19.  896.) 

Sodium  tin  (stannic)  fluoride. 
See  Fluostannate,  sodium. 

Sodium  tantalum  fluoride. 
See  Fluotantalate,  sodium. 

Sodium  tellurium  fluoride,  NaF,  TeF4. 
Decomp.  by  H20.    (Berzelius.) 

Sodium  titanium  fluoride. 
See  Fluotitanate,  sodium. 

Sodium  tungstyl  fluoride. 
See  Fluoxytungstate,  sodium. 

Sodium  uranium  fluoride,  NaF,  UF4  (?). 
Somewhat  soluble  in  H2O.    (Bolton.) 

Sodium  uranyl  fluoride. 

See  Fluoxyuranate,  sodium. 
Sodium  vanadium  sesgiufluoride. 

See  Fluovanadate,  sodium. 
Sodium  zinc  fluoride,  NaF,  ZnF2. 

Sol.  in  H2O.    (R.  Wagner.) 
Sodium  zirconium  fluoride,  5NaF,  2ZrF4. 

See  Fluozirconate,  sodium. 
Sodium  fluoride  vanadium  pentoxide. 

See  Fluoxyvanadate,  sodium. 
Sodium  hydrazide,  NH2,  NHNa. 

Decomp.  by  H2O  with  explosive  violence. 
Decomp.  by  alcohol.  (Schlenk,  B.  1915,  48. 
670.) 

Sodium  hydride,  NaH. 

Decomp.  by  H2O  and  by  acids. 

Sol.  in  fused  Na  or  Na  amalgam.  Insol.  in 
liquid  NH3.  Insol.  in  CS2,  CC14,  C6H6  and 
terebenthene.  (Moissan,  C.  R.  1902,  134. 
73.) 

Na2H4.    Decomp.  violently  by  H2O. 

Sodium  hydrosulphide,  NaSH. 

Deliquescent.    Sol.  in  H2O  and  alcohol. 

+3H2O.  Difficultly  sol.  in  H2O.  (Damoi- 
seau,  C.  C.  1885.  36.) 

Sodium  hydroxide,  NaOH. 

Very  deliquescent.  100  pts.  NaOH  under 
a  bell  jar  with  H2O  at  1&-200  absorb  552  pts. 
in  56  days.  (Mulder.) 

Very  sol.  in  H2O  with  evolution  of  much 
heat.  Sol.  in  0.47  pt.  H2O.  (Bineau,  C.  R. 
41.  509.) 


Solubility  of  NaOH  in  H2O. 

t° 

g.  per  100  g. 

Solid  phase 

Solu- 
tion 

H2O 

—  7.8 

8.0 

8.7 

Ice 

—20 

16.0 

19.1 

" 

—28 

19.0 

23.5 

Ice+NaOH.7H20 

—24 

22.2 

28.5 

NaOH.7H2O+NaOH.5H20 

—17.7 

24.5 

32.5 

NaOH.5H2O  +NaOH.4H2O 

0 

29.6 

42.0 

NaOH.4H2O 

+  5 

32.2 

47.5 

NaOH.4H2O  +NaOH.3^H2O 

10 

34.0 

51.5 

NaOH.3J^H2O 

15.5 

38.9 

63.53 

"         f.  pt. 

5 

45.5 

83.5 

NaOH.3^H2O  +NaOH.2H2O 

12 

50.7 

103.0 

NaOH.2H20  +NaOH.H2O 

20 

52.2 

109 

NaOH.H20 

30 

54.3 

119 

" 

40 

56.3 

129 

*• 

50 

59.2 

145 

" 

60 

63.5 

174 

" 

64.3 

69.0 

222.3 

f.  pt. 

61.8 

74.2 

288 

NaOH.H2O+NaOH 

80 

75.8 

313 

NaOH  (?) 

110 

78.5 

365 

14 

192 

83.9 

521 

(Pickering,  Chem.  Soc.  1893, 63. 890;  Mylius 
and  Funk,  W.  A.  B.  1900.  3.  450.  Calc.  by 
Seidell,  Solubilities,  2d  Edition,  p.  653.) 

100  g.  sat.  NaOH+Aq  at  15°  contain  46.36 
g.  NaOH.  (de  Forcrand,  C.  R.  149.  1344.) 

Sp.  gr.  and  b-pt  of  NaOH  -fAq. 


% 

Na20 

Sp.  gr. 

B.-pt. 

&> 

SP.  gr. 

B.-pt. 

4.7 
9.0 
13.0 
16.0 
19.0 
23.0 
26.0 
29.0 

1.06 
.12 
.18 
.23 
.29 
.32 
.36 
.40 

100.56° 
101.11 
102  .  78 
104  .  44 
106.66 
108  .  89 
112.78 
116.66 

31.0 
34.0 
36.8 
41.2 
46.6 
53.8 
63.6 
77.8 

1.44 
1.47 
1.50 
1.56 
1.63 
1.72 
1.85 
2.00 

120.00° 
123.89 
129.44 
137.78 
148  .  89 
204.44 
315.56 
red  heat. 

(Dalton.) 
Sp.  gr.  of  NaOH  +Aq  at  15°. 


%  Na20 

Sp.  gr. 

%  Na-20 

Sp.  gr. 

%  Na2O 

Sp.  gr. 

0.302 

1.0040 

10.879 

.1630 

21  .  154 

1.3053 

0.601 

1.0081 

11.484 

.1734 

21.758 

1.3125 

1.209 

1.0163 

12  .  088 

.1841 

21.894 

1.3143 

1.813 

1  .  0246 

12.692 

.1948 

22.363 

1.3198 

2.418 

1  .  0330 

13.297 

.2058 

22  .  967 

1  .  3273 

3.022 

1.0414 

13.901 

.2178 

23.572 

1  .  3349 

3.626 

1  .  0500 

14  .  506 

.2280 

24  .  176 

1.3426 

4.231 

1.0587 

15.110 

.2392 

24  .  780 

1.3505 

4.835 

1  .  0675 

15.714 

.2453 

25  .  385 

1  .  3586 

5.440 

1  .  0764 

16.319 

.2515 

25.989 

1.3668 

6.044 

1  .  0855 

16.923 

.2578 

26  .  594 

1.3751 

6.648 

1  .  0948 

17.528 

.2642 

27  .  200 

1  .  3836 

7.253 

1  .  1042 

18.132 

.2708 

27  .  802 

1.3923 

7.857 

1.1137 

18.730 

1  .  2775 

28.407 

1.4011 

8.462 

1  .  1233 

19.341 

1.2843 

29.011 

1.4101 

9.066 

1  .  1330 

19.954 

1.2912 

29.616 

1.4193 

9.670 

1  .  1428 

20.550 

1.2982 

30.220 

1.4285 

10.275 

1  .  1528 

(Tunnerman,  N.  J.  Pharm.  18.  2.) 


852 


SODIUM  HYDROXIDE 


Sp.  gr.  of  NaOH  +Aq. 

Sp.  gr.  of  NaOH+Aq  at  15°—  Continued. 

%  Na2O 

Sp.  gr.     %  Na2C 

Sp.  gr. 

%  Na2O    Sp.  gr. 

%  NaOH 

Sp.  gr. 

%  NaOH 

Sp.  gr. 

2.07 

1  .  02          14  .  73 

1.16 

28  16            30 

4.02 

1.04          16.73 

1.18 

29.96          .32 

7.66 

1.0868 

24.81 

1.2748 

5.89 

1.06          18.71 

1.20 

31.67           .34 

8.0 

1  .  0909 

25.3 

1  2800 

7.69 
9  43 

1.08         20.66 
1  .  10         22  .  58 

1.22 
1   24 

32.40          .35 
33  08            36 

8.34 

1.0951 

25.8 

1.2857 

11.10 

1.12         24.47 

1.26 

34^41           '.38 

8.68 

1.0992 

26.31 

1.2905 

12.81 

1.14    1     26.33 

1.28 

9.0 

1.1030 

26.83 

1.2973 

9.42 

1  .  1077 

27.31 

1  .  3032 

(Richtor.) 

9.74 

1.1120 

27.8 

1.3091 

Sp.  gr.  of  NaOH+Aq 

at 

15°. 

10.0 
10   ^ 

1.1158 
1    1  1Q"i 

28.31 

28  83 

1.3151 

% 

Sp.  gr. 

^ 

Sp.  gr. 
if  %  is 
NaOH 

% 

Sp.  gr. 

if  %  is 
NfloO 

Sp.  gr. 
NaOH 

-LU  .  «J 

10.97 
11.42 

-L  .  J.  JLi/O 

1.1250 
1  .  1294 

29^38 
30.0 

l!3272 
1.3339 

11.84 

1  .  1339 

30  57 

1  3395 

1 

1 

.015 

1.012 

32 

1 

.450 

1.351 

12.24 

1.1383 

31.22 

1.3458 

2 

1 

.020 

1.023 

33 

1 

.462 

1.363 

12  '.64 

1  .  1423 

31.85 

1.3521 

3 

1 

.043 

1.035 

34 

1 

.475 

1.374 

13.0 

.1474 

32.47 

1.3585 

4 

1 

.058 

1.046 

35 

1 

.488 

1.384 

13.55 

.1520 

33.0 

1.3642 

5 

1 

.074 

1.059 

36 

1 

.500 

1.395 

13.86 

.1566 

33.69 

1.3714 

6 

1 

.089 

1.070 

37 

1 

.515 

1.405 

14.5 

.1631 

34.38 

1.3780 

7 

1 

104 

.081 

38 

1 

.530 

1.415 

14.75 

.1662 

35.0 

1.3858 

8 

1 

119 

.092 

39 

1 

.543 

1.426 

15.0 

.1697 

35.65 

1.3913 

9 

1 

132 

.103 

40 

1 

.558 

1.437 

15.5 

.1755 

36.25 

1.3981 

10 

1 

145 

.115 

41 

1 

.570 

1.447 

15.91 

.1803 

36.86 

1.4049 

11 

1 

160 

.126 

42 

1 

.583 

1.456 

16.38 

.1852 

37.47 

1.4118 

12 

1 

175 

.137 

43 

1 

.597 

1.468 

16.77 

.1901 

38.13 

1.4187 

13 

1 

190 

.148 

44 

.610 

1.478 

17.22 

.1950 

38.8' 

1.4267 

14 

1 

203 

.159 

45 

.623 

1.488 

17.67 

.2000 

39.39 

.4328 

15 

1 

219 

.170 

46 

.637 

1.499 

17.12  • 

.2050 

40.0 

.4410 

16 

1 

233 

.181 

47 

.650 

.508 

18.58 

.2101 

40.75 

.4472 

17 

1 

245 

.192 

48 

.663 

.519 

19.0 

.2148 

41.41 

.4545 

18 

1 

258 

.202 

49 

.678 

.529 

19.58 

.2202 

42.12 

.4619 

19 

1 

270 

.213 

50 

.690 

.540 

20.0 

.2250 

42.83 

.4694 

20 

1 

285 

.225 

51 

.705 

.550 

20.59 

.2308 

43.66 

.4769 

21 

1 

300 

.236 

52 

.719 

.560 

21.0 

.2361 

44.38 

.4845 

22 

1 

315 

.247 

53 

.730 

.570 

21.42 

.2414 

45.27 

.4922 

23 

1 

329 

.258 

54 

.745 

.580 

22.0 

.2462 

46.15 

.5000 

24 

1 

341 

.269 

55 

.760 

.591 

22.64 

.2522 

46.87 

1.5079 

25 

1 

355 

.279 

56 

.770 

.601 

23.15 

.2576 

47.60 

1.5158 

26 

1 

369 

1.290 

57 

.785 

.611 

23.67 

.2632 

48.  ai 

1.5238 

27 

oo 

1 

381 

oricr 

1.300 

1O  1  f\ 

58 

Kf\ 

.800 

01  er 

.622 

£»OO 

24.24 

.2687 

49.02 

1.531 

28 
29 

1 
1 

395 
410 

.310 
1.321 

59 
60 

.815 
.830 

.633 
.643 

Hager,  Comm.  1883.) 

30 
31 

1.422 
1.438 

1.332 
1.343 

70 

1.748 

The  sp.  gr.  increases  or  diminishes  for  each 
degree  as  follows: 

(Gerlach,   Z.  anal.  8.  279,   calculated  from 

%  NaOH 

Corr. 

Schiff,  A.  107.  300 

j 

40-50 

0.00045 

Sp.  gr.  of  NaOH+Aq  at  15°. 

30-39 

0.0004 

%  NaOH          Sp.  gr. 

%  NaOH 

Sp.  gr. 

20-29 
10-19 

0  .  0003 
0.0002 

0.61 
0.9 

1.0070 
1.0105 

4.0 
4.32 

1.0435 
1.0473 

Hager,  Comm.  1883.) 

1.0 
1  2 

1.0107 

4.64 

1.0511 

Sp.  gr.  of  NaOH+Aq  at  15°. 

i!e 

l!oi77 

5^29 

.0588 

%  NaOH 

Sp.  gr. 

%  NaOH 

Sp.  gr. 

2.0 
2.36 

1.0213 
1.0249 

5.58 
5.87 

.0627 
.0667 

2.5 

1.0280 

20 

1.2262 

2.71 

1.0286 

6.21 

.0706 

5 

1.0568 

25 

1  .  2823 

3.0 

1.0318 

6.55 

.0746 

10 

1.1131 

30 

1  .  3374 

3.35 

1.0360 

6.76 

.0787 

15 

1  .  1790 

3.67 

1  .  0397 

7.31 

.0827 

(Kohlrausch,  W.  Ann.  1879.) 

SODIUM  HYDROXIDE 


853 


Sp.  gr  of  NaOH+Aq  at  20°  containing 
2  mols.  NaOH  to  100  mols.  H2O  =  1.04712. 
(Nicol,  Phil.  Mag.  (5)  16.  122.) 

Sp.  gr.  of  NaOH-f-Aq  at  15°. 


%  Na2O 

Sp.  gr. 

%  Na2O 

Sp.  gr. 

5 

1.069 

25 

1.353 

10 

1.139 

30 

1.426 

15 

1.210 

35 

1.500 

20 

1.281 

(Hager,    Adjumenta    Varia,    Leipsic,    1876.) 
Sp.  gr.  of  NaOH+Aq  at  15°. 


&s§ 

Sp.  gr. 

asS 

Sp.  gr. 

4 

Sp.  gr. 

0 

0.999180 

17 

1.188707 

34 

1.373453 

1 

.010611 

18 

1.199783 

35 

1.383815 

2 

.021920 

19 

1.210861 

36 

1.394092 

3 

.033109 

20 

1.221933 

37 

1.404279 

4 

.044317 

21 

1.233062 

38 

1.414363 

5 

.055463 

22 

1.244119 

39 

1.424353 

6 

.066602 

23 

1.255134 

40 

1.434299 

7 

.077733 

24 

1.266092 

41 

1.444161 

8 

.088856 

25 

1.277063 

42 

1.453929 

9 

.099969 

26 

1  .  287990 

43 

1.463623 

10 

.111069 

27 

1.298877 

44 

1.473249 

11 

.  122165 

28 

1.309708 

45 

1.482850 

12 

.  133250 

29 

1.320496 

46 

1.492406 

13 

.  144353 

30 

1.331213 

47 

1.501927 

14 

.  155450 

31 

1.341879 

48 

1.511412 

15 

1.166538 

32 

1.352472 

49 

1.520868 

16 

1.177619 

33 

1.362991 

50 

1.530282 

(Pickering,  Phil.  Mag.  1894,   (5)  37.  373.) 

Sp.  gr.  of  a  N  solution  of  NaOH+Aq  at 
18°/18°  =  1.0418.  (Loomis,  W.  Ann.  1896,  60. 
550.) 

Sp.  gr.  of  NaOH+Aq. 

%NaOH  8.73  3.67  3.82 

Sp.  gr.  20°/20°        1.0968       1.0416        1.0464 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 

19.  272.) 

Sp.  gr.  of  NaOH+Aq  at  t°.  H2O  at  4°  =  1. 
The  solutions  contained  a  small  amount 
of  Na2CO3. 


60 


%  NaOH 


22.57 
20.04 
17.04 
14.16 
10.92 


%  Na2C03 


0.61 
0.48 
0.35 
0.38 
0.36 


Sp.  gr. 


.2312 
.2026 
.1692 
.1374 
.1020 


Sat.  NaOH+Aq  boils  at  215.5°.  (Grif- 
fiths.) 

Sat.  NaOH+Aq  boils  at  310°.  (Gerlach, 
Z.  anal.  26.  427.) 

NaOH+Aq  of  1.500  sp.  gr.  contains  36.8% 
NaOH  and  boils  at  130°. 

B.-pt.  of  NaOH+Aq  containing  pts.  NaOH 
to  100  pts.  H2O. 


B.-pt. 

Pts.  NaOH 

B.-pt. 

Pts.  NaOH 

105° 

17    ' 

210° 

425.5 

110 

30 

215 

475.5 

115 

41 

220 

526.3 

120 

51 

225 

583.3- 

125 

60.1 

230 

645.2 

130 

70.1 

235 

714.3 

135 

81.1 

240 

800 

140 

93.5 

245 

888.8 

145 

106.5 

250 

1000 

150 

120.4 

255 

1142.8 

155 

134.5 

260 

1333.3 

160 

150.8 

265 

1534 

165 

168.8 

270 

1739.1 

170 

187 

275 

2000 

175 

208.3 

280 

2353 

180 

230 

285 

2857 

185 

254.5 

290 

3571.4 

190 

281.7 

300 

4651  .  1 

195 

312.3 

305 

6451.6 

200 

345 

310 

10526.3 

205 

380.9 

314 

22222.2 

(Gerlach,  Z.  anal.  26.  463.) 

Insol.  in  liquid  NH3.     (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Sp.  gr.  of  Na2CO3+NaOH+Aq  at  11.5°. 
H2Oat4°  =  l. 


%  Na2COs 

%  NaOH 

Sp.  gr. 

3.845 
3.171 
2.204 
1.642 
0.2686 

14.10 
13.63 
12.51 
10.17 
16.64 

1.196 
1.182 
1.164 
1.136 
1.186 

(Wegscheider  and  Walter,  M.  1905,  26.  693.) 

Sp.  gr.  of  Na2CO3+NaOH+Aq  at  t°.    H2O 
at4°  =  l. 


60C 


%  Na2CO3 


15.38 

13.79 

12.10 

9.965 

9.47 

7.69 


%  NaOH 


10.63 
9.52 
8.29 
6.86 
6.70 
5.22 


Sp.  gr. 


1.2621 
.2302 
.1952 
.1594 
.1521 
.1158 


80 


22.81 
14.01 


0.55 
0.42 


.2207 
.1232 


80C 


15.26 
9.48 


11.14 
6.93 


.2510 
.  1417 


(Wegscheider  and  Walter,  M.  1905,  26.  691.) 


(Wegscheider  and  Walter,  M.  1905,  26.  692.) 


854 


SODIUM  HYDROXIDE 


Solubility  of  NaOH+Na3SbS4  at  30°. 

Solubility  of  NaI+2H2O  in  100  pts.  at  t°. 

%  NaOH 

%  NasSbS4 

Solid  phase 

Pts. 

' 

Pts. 

Pts. 

Nal 

Nal 

Nal 

0 
9.9 

27.1 
13. 

Na3SbS4,  9H2O     - 
it 

-  17 

149.4 

15 

173.7 

45 

215.6 

24.8 

5.9 

(t 

-15 

150.3 

20 

178.7 

50 

227.8 

32.9 

10.5 

u 

-   5 

155.4 

25 

184.2 

55 

241.2 

42.6 

16.4 

(( 

0 

158.7 

30 

190.3 

60 

256.8 

47.2 
49.5 

17.7 
9.1 

"  +NaOH,  H2O 
NaOH,  H2O 

5 
10 

163.6 
168.6 

35 

40 

197.0 
205.1 

65 

278.4 

54.3 

(Coppet,  A.  ch.  (5)  60.  424.) 

(Donk,  Chem.  Weekbl.  1908,  6. 529,  629,  767.) 

Easily  sol.  in  alcohol  or  wood  spirit;  sol.  in 
fusel-oil.  Sol.  in  an  aqueous  solution  of 
mannite.  (Favre,  A.  ch.  (3)  11.  76.) 

Easily  sol.  in  glycerine. 

Sol.  to  a  certain  extent  in  ether. 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate  (Naumann, 
B.  1904,  37.  3602);  benzonitrile.  (Naumann, 
B.  1914,  47.  1370.) 

+H2O.  100  g.  solution  in  H2O  sat.  at  25° 
contain  42  g.  Na2O.  (Schreinemakers,  Arch. 
Ne'er.  Sc.  1910,  (2)  16.  81.) 

Mpt.  64.3°.    (See  above.) 

+lVsH2O.  (Cripps,  Pharm.  J.  Trans.  (3) 
14.  833.) 

+2H2O.    See  above. 

+3Y2H2O.    Deliquescent.    Sol.  in  H2O  with 
absorption    of    much    heat.      Melts    at    6 
(Hermes.) 

Mpt.  15.5°.    (See  above.) 

+4,  5  and  7H2O.    (See  above.) 

The  composition  of  the  hydrates  formed 
by  NaOH  at  different  dilutions  is  calculated 
from  determinations  of  the  lowering  of  the 
fr.-pt.  produced  by  NaOH  and  of  the  con- 
ductivity and  sp.  gr.  of  NaOH+Aq.  (Jones 
Am.  Ch.  J.  1905,  34.  336.) 

Sodium  perhydroxide,  NaO2H. 

"Natryl  hydroxide." 

Decomp.  by  H2O.  Sol.  in  cold  alcoholic 
acetic  acid.  (Tafel,  B.  1894,  27.  2300.) 

Sodium  iodide,  Nal,  and  +2H2O. 

Solubility  of  Nal  and  of  NaI+2H2O  in 
H2O  differ.  Below  65°,  NaI+2H2O  usually 
separates  out,  and  above  that  temp.  Nal 
separates. 

Solubility  of  Nal  in  100  pts.  H2C  at  t°. 


t° 

Pts. 
Nal 

t° 

Pts. 
Nal 

t 

Pts. 
Nal 

71.3 
74.1 
81.6 
86.4 

294.4 
295.3 
296.8 
298.3 

92.4 
97.1 
101.7 
110.7 

300.2 
300.3 
302.5 
306.2 

124.7 
132.5 
138.1 

317.5 
317.3 

319:2 

Solubility  is  represented  by  a  straight  line 
of  the  formula  S  =  264.  19+0.3978t. 

If  solubility  S  =  pts.  Nal  in  100  pts,  solu- 
ion,  S  =  61.3+0.1712t  from  0°  to  80°;  S  = 
75+0.0258t  from  80°  to  160°.    (Etard,  C.  R. 
98.  1432.) 

NaI+2H2O  is  sol.  in  0.55  pt.  H20  at  15°. 
Eder,  Dingl.  221.  89.) 

100  pts.  Nal+Aq  at  18-19°  contain  62.98 
pts.  Nal.    (v.  Hauer,  J.  pr.  98.  137.) 

100  pts.  H2O  dissolve  at: 
0°  20°  40° 

158.7          178.6        208.4 


60° 
256.4  pts.  Nal, 


80°  100°          120°          140° 

303  312.5        322.5        333.3  pts.  Nal. 

(Kremers,  Pogg.  97.  14.) 

Transition  pt.  for  NaI+2H29  to  Nal  is 
64.3°,  and  sat.  solution  containing  74.4% 
Nal.  (Panfilofif,  J.  Russ.  Phys.  Chem.*  Soc. 
1893,  25.  162.) 

100  g.  H2O  dissolve  172.4  g.  Nal  at 
15°,  and  sp.  gr.  of  sat.  solution  =  1.8937. 
(Greenish,  Pharm.  J.  1900,  65.  190.) 

100  g.  solution  of  NaI+2H2O  sat.  at  30° 
contains  65.5  g.  anhyd.  Nal.  (Cocheret, 
Dissert.  1910.) 

Sp.  gr.  of  Nal+Aq  at  19.5°  containing: 

5  10  15  20  25  30  %  Nal, 
1.040  1.082  1.128  1.179  1.234  1.294 

35        40        45        50        55        60  %  Nal. 
1.360  1.432  1.510  1.60     1.70     1.81 
(Gerlach,  Z.  anal.  8.  285.) 

Sat.  solution  boils  at  141°. 

Sol.  in  liquid  SO2.  (Walden,  B.  1899,  32. 
2864);  POC13.  (Walden,  Z.  anorg.  1900,  25- 
212.) 

Very  easily  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  829.) 

Sol.  in  12.0  pts.  absolute  alcohol;  in  360 
pts.  ether.  (Eder,  Dingl.  221.  89.) 

Sol.  in  3  pts.  90%  alcohol.    (Hager.) 

100  pts.  absolute  methyl  alcohol  dissolve 
77.7  pts.  Nal  at  22.5°;  ethyl  alcohol,  43.1  pts. 
(de  Bruyn,  Z.  phys.  Ch.  10.  783.) 

Very  sol.  in  abs.  methyl  alcohol  and  is  not 
pptd.  therefrom  on  the  addition  of  a  large 
volume  of  abs.  ether,  while  wet  ether  produces 
immediate  separation.  (Loeb,  J.  Am.  Chem. 
Soc.  1905,  27.  1020.) 


SODIUM  IODIDE 


855 


Solubility  of  Nal  in  ethyl  alcohol, 
(g.  Nal  in  100  g.  alcohol.) 

Solubility  in  methyl  alcohol  +  ethyl  alcohol 
at  25°. 
P  =  %  methyl  alcohol  in  the  solvent. 
G  =  g.  Nal  in  10  ccm.  of  the  solution. 
S  =  Sp.  gr.  of  the  sat.  solution  at  25°. 

t° 

Nal 

t° 

Nal 

10 
30 
50 
80 
100 
120 
160 
180 

43.77 
44.25 
44.50 
45.0 
45.1 
45.2 
45.0 
44.3 

200 
220 
230 
240 
250 
255 
260 
261.5* 

42.3 
38.5 
36.2 
32.7 
26.2 
21.0 
10.8 
8.6 

p 

G 

S  25°/4° 

0.00 
4.37 
10.40 
41.02 
80.69 
84.77 
91.25 
100.00 

3.515 
3.768 
3.971 
4.598 
5.744 
5.892 
6.110 
6.322 

1.0806 
1.1029 
1.1123 
1.1742 
1.2741 
1.2886 
1.3056 
1.3250 

""Critical  temp,  of  solution. 
(Tyrer,  Chem.  Soc.  1910,  97.  626.) 

(Herz  and  Kuhn,  Z.  anorg.  1908,  60.  154.) 

100  g.  sat.  solution  of  Nal  in  ethyl  alcohol 
at  30°  contains  30.9  g.  (Cocheret,  Dissert, 
1910.) 


Solubility  in  mixtures  of  methyl  and  propyl 

alcohol  at  25°. 

P  =  %  propyl  alcohol  in  the  solvent. 
G  =  g.  Nal  in  10  ccm.  of  the  solution. 
S=Sp.  gr.  of  the  sat.  solution. 


Solubility  in  ethyl  alcohol  +Aq  at  30°. 

P 

G 

S  25°/4° 

6OOO 

%  Nal 

%  alcohol 

Solid  phase 

11.11 

.322 
5.845 

.3250 
.2853 

65.52 

0 

Nal,  2H2O 

(( 

•      23.8 
65.2 

5.464 
4.071 

.2528 
.138 

64 

3.40 

ff 

91.8 

2.914 

.0420 

54.2 

r*  A 

18.5 

1  Q    Q 

(i 

93.75 

2.649 

.0178 

54 

lo.o 

oo     er 

fi 

100.00 

2.411 

0.9968 

48.8 

28.5 

42.35 
38.5 

41.7 
53.2 

K 
it 

(Herz  and  Kuhn,  Z.  anorg.  1908,  60.  156.) 

37.91 
37.49 
35.65 

54.7 
55.37 
59.24 

(i 

Nal,  2H20+NaI 
Nal 

Solubility  in  mixtures  of  propyl  and  ethy 
alcohol  at  25°. 

33.24 

61.78 

a 

P  =  %  propyl  alcohol  in  the  solvent. 

30.90 

68.70 

(l 

G  =  g.  Nal  in  10  ccm.  of  the  solution. 
S  =  Sp.  gr.  of  the  sat.  solution. 

(Cocheret,  Dissert.  1911.) 

P 

G 

S  25°/4° 

0 

3.515 

1.0806 

At  room  temp.  1  pt.  by  weight  is  sol  in: 

8.1- 
17.85 

3.460 
3.405 

1.0732 
1.0720 

1.2  pts.  methyl  alcohol  D15  0.7990. 

56.6 

2.841 

1.0276 

1.7      "  ethyl            "     D15  0.8100. 

88.6 

2.613 

1.0130 

3.8      "  propyl          "     D15  0.8160. 

91.2 

2.588 

1.0104 

(Rohland,  Z.  anorg.  1898,  18.  325.) 

95.2 
100 

2.474 
2.411 

1.0020 
0.9968 

100  g.  methyl  alcohol  dissolve  90.35  g. 
Nal  at  25°. 

100  g.  ethyl  alcohol  dissolve  46.02  g.  Nal  at 
25°. 

100  g.  propyl  alcohol  dissolve  28.22  g. 
Nal  at  25°. 

100  g.  isoamyl  alcohol  dissolve  16.30  g. 
Nal  at  25°. 

(Turner  and  Bissett,  Chem.  Soc.  1913,  103. 
1909.) 


(Herz  and  Kuhn,  Z.  anorg.  1908,  60.  159.) 

Sol.  in  normal  propyl  alcohol.  (Loeb,  J. 
Am.  Chem.  Soc.  1905,  27.  1020.) 

28.74  g.  are  sol.  in  100  g.  propyl  alcohol. 
(Schlamp,  Z.  phys.  Ch.  1894,  14.  276.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3789.) 

Sol.  in  ethyl  acetate.  (Casaseca,  C.  R.  30. 
821.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,43.314.) 


856 


SODIUM  TIN  IODIDE 


SI.  sol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1369.) 

Solubility  in  organic  solvents  at  t°. 

C=pts.  by  wt.  of  Nal  in  100  ccm.  of  the 
sat.  solution. 

L=no.  of  liters  which  at  the  saturation 
temp,  hold  in  solution  1  mol.  Nal. 


Solvent 

t 

C 

L 

Furfurol 

25 

25.10 

0.597 

Acetonitrile 
it 

25 
0 

18.43 
22.09 

0.813 
0.679 

Propionitrile 
(t 

25 
0 

6.230 
9.091 

2.406 
1.649 

Nitromethane 

(( 

25 
0 

0.478 
0.339 

31.36 
44.27 

(Walden,  Z.  phys.  Ch.  1906,  65.  718.) 

Very  sol.  in  acetone.    (Walden.) 
+5H2O.    Transition  point  of  NaI+5H2O 
to  NaI+2H2O  is  -13.5°,  and  sat.  solution 
contains  60.2%   Nal.     (Panfiloff,   J.   Russ. 
Phys.  Chem.  Soc.  1893,  25.  162.) 

Sodium  tin  (stannous)  iodide,  Nal,  SnI2. 

Very  sol.  in  H2O.  When  treated  with  little 
H2O,  Nal  is  dissolved  out,  but  a  larger  amt. 
of  H2O  dissolves  it  completely.  (Boullay,  A. 
ch.  (2)  34.  375.) 

Sodium    zinc    iodide,    2NaI,    ZnI2+3H2O. 

Deliquescent. 

NaZnI3+2H2O.  Very  hydroscopic. 
(Ephraim,  Z.  anorg.  1910,  67.  383.) 

Sodium  nitride, 

Decomp.  by  heat.  (Franz  Fisher,  B.  1910, 
43.  1468.) 

Sodium  sw&oxide,  Na3O. 

Decomp.  by  H2O.  (de  Forcrand,  C.  R. 
1898,  127.  365.) 

Sodium  oxide,  Na2O. 

Very  deliquescent,  and  sol.  in  H2O  with 
evolution  of  heat. 

See  Sodium  hydroxide. 

Sodium  peroxide,  Na2O2. 

Deliquescent,  and  very  sol.  in  H2O  with 
partial  decomp. 

Solution  decomp.  on  boiling. 

Cryst.  with  2H2O,  and  8H2O.  (Fairley, 
Chem.  Soc.  1877.  125.) 

Forms    hydrate    Na2O2(OH)4+4H2O. 

Easily  sol.  in  H2O  or  dil.  acids  without 
decomp.  (Schone,  A.  193.  241.) 


Sodium  peroxide  carbonate,  Na2CO4. 

Easily  decomp.  (Woffenstein,  B.  1908. 
41.  285.) 

Sodium    peroxide    decarbonate,    Na2C2O6. 

Easily  decomp.  (Woffenstein,  B.  1908, 
41.  287.) 

Sodium  Znoxide,  NaO3. 

Sol.  in  H2O  forming  a  solution  of  Na2O2. 
(Joannis,  C.  R.  1893,  116.  1371.) 

Sodium  fnoxide  carbonate,  Na2COfi. 
(Woffenstein,  B.  1908,  41.  296.) 

Sodium  trioxide  bicarbonate,  NaHCO4. 

Two  isomeric  modifications.  (Woffen- 
stein, B.  1908,  41.  390.) 

Sodium  dioxide  hydrate,  NaO.OH. 

See  Sodium  perhydroxide. 

Isomeric  with  Tafel's  sodyl  hydroxide. 
OrNa.OH.  (B.  27,  2297.) 

Insol.  in  alcohol. 

Very  unstable.  (Woffenstein,  B.  1908, 
41.  290.) 

Sodium  phosphide,  NaP5. 

Easily  decomp.  by  H2O.  (Hugot,  C.  R. 
1895,  121.  208.) 

Sodium  hydrogen  phosphide,  NaH2P. 

Decomp.  by  H20.  (Joannis,  C.  R.  1894, 
119.  558.) 

Na3H3P2.  Decomp.  by  acids  and  H2O. 
(Hugot,  C.  R.,1898,  126.  1721.) 

Sodium  selenide,  Na2Se. 

Very  deliquescent.  Decomp.  by  H2O. 
(Uelsmann,  A.  116.  127.) 

Insol.  in  liquid  NH3;  sol.  in  air  free  H2O 
to  a  colorless  liquid.  (Hugot,  C.  R.  1899, 
129.  299.) 

Cryst.  with  16H2O,  9H2O,  and  9/2H2O. 
(Fabre,  C.  R.  102.  613.) 

+  10H2O.  Very  sol.  in  H2O;  very  unstable 
in  the  air.  (Clever,  Z.  anorg.  1895,  10.  145.) 

Sodium  diselenide,  Na2Se2. 
(Jackson,  B.  7.  1277.) 

Sodium  tfnselenide,  Na2Se3. 

Sol.  in  H2O.  (Mathewson,  J.  Am.  Chem. 
Soc.  1907,  29.  873.) 

Sodium  Aeoxiselemde,  Na2Se. 

Sol.  in  H2O.  (Mathewson,  J.  Am.  Chem. 
Soc.  1907,  29.  873.) 

Sodium  raonosulphide,  Na2S. 

Sol.  in  H2O.  Much  less  sol.  in  alcohol  than 
in  H2O.  Insol.  in  ether.  (Roussin.) 


STANNIC  ACID 


857 


+5H20.   Tr.  pt.  from  Na2S+5^H2O,  94°. 


The   sat.    solution    contains:  —  • 
28.48%  anhydrous  salt  at  50 


29.27 
29.92 
31.38 
33.95 
37.20 


55° 
60° 
70° 
80° 
90° 


Labile  from  48.9-91.5°;  stabile  from  91.5- 
€6°. 
(Parravano  and  Fornaini,  C.  C.  1908,  I.  5.) 

+6H2O.  Less  efflorescent  than  with  9H2O. 
Sol.  in  H2O  and  alcohol. 

The  sat.  solution  contains: — 

26 . 7  %  anhydrous  salt  at  50° 
28.1  "  "     "60° 

30.22  "  "     "70° 

32.95  "  "     "80° 

36.42  "  "     "90° 

Tr.  pt.  to  Na2S+5MH2O,  91.5°. 
(Parravano  and  Fornaini.) 

+9H2O.  Efflorescent.  Much  less  sol.  in 
alcohol  than  H2O.  When  dissolved  in  H2O, 
temp,  sinks  from  +22  to— 6.1°.  (Finger, 
Pogg.  128.  635.) 

The  sat.  solution  contains: — • 

9.34%  anhydrous  Na2S  at  —10° 
13.36  '  '     "  +10° 

14.36  '  '      '      15° 

15.30  '  '      '      18° 

16.2  '  '      '      22° 

17.73  '  '      '      28° 

19.09  '  '      '      32° 

20.98  '  '      '      37° 

24.19  '  '      '      45° 

Tr.  pt.  to  Na2S+5^H2O,  48.9°. 
(Parravano  and  Fornaini.) 

Sodium  cfo'sulphide,  Na2S2. 
Sol.  in  H2O  and  alcohol. 
+5H2O.  Not  efflorescent. 

Sodium  bisulphide,  Na2S3. 

Sol.  in  H2O  with  decomp. 

Cryst.  with  3H2O  from  an  alcoholic  solu- 
tion. (BSttger,  A.  223.  355.) 

Sodium  tefrasulphide,  Na2S4+6H2O. 

Very  deliquescent,  and  sol.  in  H2O.  Diffi- 
cultly sol.  in  absolute  alcohol.  Insol.  in  ether. 
(Schone.) 

+8H2O.    Efflorescent.    (Bottger.) 

Sodium  pentasulphide,  Na2S5+6H2O. 

Sol.  in  H2O.     (Schone.) 

Sol.  in  alcohol. 

+8H?O.    (Bottger.) 

Solution  is  easily  decomp.  by  warming. 
(Jones,  Chem.  Soc.  37.  461.) 


Sodium  tellurium  sulphide. 
See  Sulphotellurate,  sodium. 

Sodium  stannic  sulphide. 
See  Sulphostannate,  sodium. 

Sodium  yttrium  sulphide,  Na2S,  Y2S3. 

Decomp.  by  dil.  acids,  even  by  HC2H3O2  + 
Aq.  (Duboin,  C.  R.  107.  243.) 

Sodium  zinc  sulphide,  Na2S,  3ZnS. 

Not  so  stable  as  the  corresponding  K  salt. 
(Schneider,  J.  pr.  (2)  8.  29.) 

Sodium  sulphoselenide,  Na2SSe2+5H2O. 

Hydroscopic,  and  decomp.  in  the  air.  (Mes- 
singer,  B.  1897,  30.  806.) 

Sodium  telluride,  Na2Te. 

Sol.  in  H2O.  (Demarcay,  Bull.  Soc.  (2) 
40.  99.) 

Sodium  fritelluride,  Na2Te3. 

Sol.  in  H2O. 

Sol.  in  liquid  NH3.  (Hugot,  C.  C.  1899, 
II.  580.) 

Stannic  acid,  H2SnO3. 

Insol.  in  H2O.  Sol.  in  HC1,  and  H2SO4+ 
Aq,  even  when  dil.  (Fremy.)  Easily  sol.  in 
acids,  from  which  solution  it  may  be  pptd.  by 
dilution  or  boiling.  While  moist  it  is  sol.  in 
HNO3+Aq,  but  gradually  separates  on  stand- 
ing, and  coagulates  at  once  when  heated  to 
50°.  If  NH4NO3  be  added  to  the  solution,  it 
remains  clear  at  ord.  temp.  (Berzelius.) 

Easily  sol.  in  HNO3+Aq,  when  previously 
treated  with  NH4OH+Aq.  (The'nard.) 

Easily  sol.  in  KOH+Aq,  but  addition  of 
large  excess  ppts.  K2SnO3,  insol.  in  KOH  + 
Aq. 


Easily  sol.  in  NaOH+Aq,  and  not  pptd.  by 
an  excess  of  that  reagent.  (Barfoed,  J.  B. 
1867.  267.) 


SI.  sol.  in  NH4OH+Aq  or  (NH4)2CO3+Aq. 

Completely  sol.  in  K2CO3+Aq,  but  not  in 
Na2CO3+Aq. 

Insol.  in  alkali  hydrogen  carbonates  or 
NH4Cl+Aq. 

Sol.  in  alkali  sulphides +Aq.     (Berzelius.) 

Sol.  in  triethyltoluenyl  ammonium  hy- 
drate+Aq. 

Not  pptd.  by  NH4OH+Aq  in  presence  of 
Na  citrate +Aq. 

SnO2,  2H2O.     (Weber,  Pogg.  122.  358.) 

"  a-Orthostannic  acid."  Easily  sol.  in 
HCl+Aq.  (Neumann,  M.  12.  515.) 

H10Sn5015  (?) 

Metastannic  acid.  Insol.  in  H2O,  HNO3, 
or  H2SO4+Aq.  Insol.  in  HCl+Aq,  but 
converted  thereby  into  metastannic  chloride, 
which  dissolves  after  excess  of  HC1  has  been 
removed.  (Fresenius.)  Insol.  in  HCl+Aq  of 
sp.  gr.  1.1.  (Barfoed.)  Sol.  in  large  amount 


858 


STANNIC  ACID 


of  cone.  HCl+Aq.  (Allen,  Chem.  Soc.  (2)  10. 
274.) 

In  contact  with  HCl+Aq,  metastannic 
acid  is  converted  into  stannic  acid.  (Bar- 
foed.) 

Insol.  in  HNO3+Aq  even  after  treatment 
with  NH4OH+Aq. 

Insol.  in  NH4OH+Aq. 

Sol  in  KOH  or  NaOH+Aq  with  formation 
of  metastannates,  which  are  insol.  in  dil. 
NaOH+Aq,  but  sol.  in  H2O  or  KOH+Aq, 
therefore  KOH+Aq  dissolves  metastannic 
acid,  while  NaOH+Aq  does  not,  but  if  the 
clear  solution  in  KOH+Aq  is  treated  with  a 
large  excess  of  that  reagent,  a  further  pptn. 
occurs.  (Barfoed,  J.  pr.  101.  368.) 

Insol.  in  K2CO3+Aq  (Rose);  alkali  car- 
bonates+Aq.  (Fremy.) 

Insol.  in  NH4Cl+Aq  even  after  long  boil- 
ing. 

Sol.  in  Fe(NO3)3+Aq  containing  HNO3. 
(Lepez  and  Storch,  W.  A.  B.  98,  2b.  270.) 

Also  in  Cr(NO3)3+Aq,  but  not  in  Ce(NO3)3, 
Al(NOg),,  Co(NO3)2+Aq,  etc.  (L.  and  S.) 

A  colloidal  metastannic  acid  sol.  in  H2O  can 
be  obtained.  (Lepez  and  Storch.) 

According  to  Weber  (Pogg.  122.  358), 
stannic  and  metastannic  acids  are  only  differ- 
ent hydrates  of  same  oxide,,  and  it  is  not  a 
case  of  allotropic  modification. 

Colloidal.  H2SnO3  in  colloidal  state  can  be 
obtained  in  aqueous  solution  containing 
5.164  g.  SnO2  in  a  litre.  This  solution  is 
coagulated  by  HNO3+Aq  only  when  in 
great  excess;  easily  by  dil.  H2SO4+Aq, 
but  not  by  cone.  HCl+Aq.  NH4OH+Aq  in 
large  excess  causes  coagulation;  also  NH4C1, 
NaOH,  NaCl,  Na2S04,  etc.  (Schneider,  Z. 
anorg.  6.  83.) 

Pamstannic   acid,    H2Sn5On+3H2O. 
(Engel,  C.  R.  1897,  126.  711.)    ' 

Stannates. 

Stannates  of  alkali  metals  are  sol.  in  H2O; 
others  are  insol.  All  metastannates,  except- 
ing Na,  K,  and  NH4  salts,  are  insol.  in  H2O. 
(Fremy,  A.  ch.  (3)  12.  474.) 

Ammonium  stannate,  (NH4)2O,  2SnO2. 

Sol.  in  H2O.  Insol.  in  dil.  NH4OH+Aq. 
(Berzelius.) 

+zH2O.     (Moberg,  1838.) 

Ammonium      cupric      stannate,      (NH4)2O, 

CuSnO3+2H2O. 

Insol.  in  H2O.  Sol.  in  acids.  (Ditte,  C.  R. 
96.  701.) 

Barium  stannate,  BaSnO3+6H2O. 
Ppt.    Sol.  in  HCl+Aq.     (Moberg.) 
Ba2SnO4+10H2O.    Insol.  in  H2O.    Sol.  in 

acids.    (Ditte,  C.  R.  95.  641.) 


Calcium  stannate,  CaSnO3+4H2O. 

Ppt.    (Moberg.) 

+5H2O.  Insol.  in  H2O.  Sol.  in  acids. 
(Ditte,  C.  R.  96.  701.) 

2CaO,  SnO2.  (Zulkowski,  Chem.  Ind. 
1901,  24.  422.) 

Cobaltous   stannate,   CoSnO3+6H2O. 
Insol.  in  H2O.    Sol.  in  acids.    (Ditte.) 

Cupric  stannate,  CuSnO3+3H2O. 
(Moberg.) 
+4H2O.    Insol.  in  H2O.      (Ditte.) 

Cuprous    stannous    stannate,    Cu2O,    3SnO, 

SnO2+5H2O. 

Slowly  decomp.  by  dil.  acids,  and  NH4OH  + 
Aq;  completely  decomp.  by  cone,  acids. 
(Lenssen,  J.  pr.  79.  90.) 

Gold  (aurous)  stannate. 
See  Gold  purple. 

Lead  stannate,  RbSn(OH)6. 

Ppt.  (Bellucci,  Chem.  Soc.  1905,  88. 
(2)  40.) 

Lithium  stannate  teatungstate,  2Li2O,  SnO2, 

6WO3  =  Li2SnO3,  Li2W6O19. 
Insol.   in  H2O.      (Knorre,   J.   pr.    (2)   27. 

49.) 

Magnesium  stannate. 
Ppt.     (Moberg.) 

Manganous  stannate. 
Ppt.    (Moberg.) 

Mercurous    stannate,    Hg2SnO3+5H2O. 
Ppt. 

Mercuric  stannate,  HgSnO3+6H2O. 
Ppt.    (Moberg,  J.  pr.  28.  231.) 

Nickel  stannate,  NiSnO3+5H2O. 

Insol.  in  H2O.  Sol.  in  acids.  (Ditte,  C.  R. 
96.  701.) 

Platinous  sodium  stannous  stannate,  2PtO, 

Na2O,  SnO,  SnO2(?). 
(Schneider,  Pogg.  136.  105.) 

Platinous    stannous    stannate,    PtO,    2SnO, 

SnO2. 

Decomp.  by  cone,  alkalies.  (Schneider,) 
Pogg.  136.  105.) 

Potassium  stannate,  K2SnO3+3H2O. 

100  pts.  H2O  dissolve  106.6  pts.  at  10°, 
solution  has  sp.  gr.  =  1.618;  100  pts.  dissolve 
110.5  pts.  at  20°,  solution  has  sp.  gr.  =  1.627. 
(Ordway,  Sill.  Am.  J.  (2)  40.  173.) 


STRONTIUM  AMIDE 


859 


Very  si.  sol.  in  cone.  KOH+Aq. 

Insol.  in  KCl+Aq.    (Fremy.) 

Insol.  in  alcohol. 

Pptd.  from  aqueous  solution  by  the  ad- 
dition of  any  soluble  salt,  especially  those 
of  K,  Na,  and  NH4  (Fremy);  by  NH4C1,  but 
not  by  KC1  or  NaCl  (Ordway). 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  329.) 

Potassium  wetastannate,  K2O,  10SnO2. 

K2O,  7SnO2+3H2O.  Sol.  in  H2O.  Solu- 
tion gelatinises  on  heating.  (Rose.) 

K2O,  6SnO2+5H2O.  Sol.  in  H2O,  but  loses 
its  solubility  by  drying.  (Fremy,  A.  ch.  (3) 
12.  475.) 

K2O,  5Sn02+4H2O.  Completely  sol.  in 
H2O.  Insol.  in  alcohol.  (Fremy,  A.  ch.  (3) 
23.  396.) 

K2O,     3SnO2+3H2O.       Deliquescent. 
(Fremy.) 

Silver  stannate,  Ag2SnO3. 

Insol.  in  H2O.  Unacted  upon  by  NH4OH 
or  HCl+Aq.  (Ditte.) 

Silver  (argentous)  stannous  stannate  (?), 
Ag4O,  SnO,  3SnO2+3H2O  (?). 

Cold  dil.  HNOg+Aq  slowly  dissolves  all 
Ag,  hot  HNO3+Aq  rapidly. 

Easily  sol.  in  boiling  cone.  H2SO4.  (Schulze, 
J.  B.  1857.  257.) 

Sodium  stannate,  Na2SnO3+3H2O. 

More  easily  sol.  in  cold  than  in  hot  H2O. 

(Fremy.) 
Sol.  in  2  pts.  H2O  at  20°  and  100.°    (Mar- 

ignac.) 

100  pts.  H2O  dissolve  67.4  pts.  at  0°,  61.3 

pts.  at  20°,  and  solutions  have  sp.  gr.  =  1.472 

and  1.438  at  15.5°.     (Ordway,  Sill.  Am.  J. 

(2)  40.  173.) 
Pptd.  from  Na2SnO3+Aq  by  salts  of  K,  Na, 

and  NH4. 

Insol.  in  acetone.    (Naumann,  B.  1904,  37. 

4329.) 

+4H2O.     (Prandtl,  B.  1907,  40.  2129.) 
+8H2O.     (Haeffely,  J.  B.  1857.  650.) 
+9H2O.    (Jones,  C.  C.  1865.  607.) 
+  10H2O.     Very   efflorescent.      (Scheurer- 

Kestner,  Bull.  Soc.  (2)  8.  389.) 

Sodium  raetastannate,  Na2O,  9SnO2  + 
8H2O. 

Sol.  in  H2O.  Insol.  in  NaOH+Aq  or 
alcohol.  (Barfoed,  J.  B.  1867.  267.) 

Na2O,  5SnO2.  Very  difficultly  sol.  in  H2O. 
(Fremy,  A.  ch.  (3)  23.  399.) 

Insol.  in  KOH+Aq. 

+8H2O.    (Haeffely,  Chem.  Gaz.  1855.  59.) 

Sodium  stannate  vanadate, 

Na2SnO3,  3Na3VO4+32H2O. 

Na2SnO3,  4Na3VO4+48H2O. 

Na2SnO3.  5Na3VO4+64H2O. 

Na2SnO3,  6Na3VO4+80H2O.     (Prandtl, 
B.   1907,  40.  2128.) 


Strontium  stannate,  3SrO,  2SnO2  +  10H2O. 

Ppt.  Insol.  in  H2O.  Sol.  in  acids.  (Ditte, 
C.  R.  96.  641.) 

SrSn(OH)6.  (Belluci,  Chem.  Soc.  1905, 
88  (2)  40.) 

Tin  (stannous)  stannate,  SnO,  6Sn02+5H2O. 

Insol.  in  H2O.  Decomp.  by  HNO3+Aq 
into  metastannic  acid.  (Schiff,  A.  120.  53.) 

Sol.  in  HCl+Aq,  and  in  KOH+Aq. 

Tin  (stannous)  wetastannate,  SnO,  7SnO2. 

SnO,  6SnO2+9H2O.  Sol.  in  KOH+Aq  or 
in  HCl+Aq.  (Fremy.) 

+4H20.    (Schiff.) 

Zinc  stannate,  ZnSnO8+2H2O. 

Ppt.    (Moberg,  1838.) 

3ZnO,2SnO2+10H2O.  Insol.  in  H2O.  Sol. 
in  acids.  (Ditte.) 

Perstannic  acid,  H2Sn2O7. 
See  Perstannic  acid. 

Stannophosphomolybdic  acid. 

Ammonium  stannophosphomolybdate, 

3(NH4)2O,    4SnO2,    3P2O6,     16MoO3+ 
28H2O. 
Quite  insol.  even  in  boiling  H2O.    (Gibbs, 

Am.  Ch.  J.  7.  392.) 

Stannophosphotungstic  acid. 

Ammonium  stannophosphotungstate, 

2(NH4)2O,  2SnO2,  P2O6,  22WO3  +  15H2O. 
Precipitate.      SI.    sol.    in    boiling    H2O. 
(Gibbs,  Am.  Ch.  J.  7.  319.) 

Stannosulphuric  acid. 
See  Sulphate,  stannic. 

Stibine. 
See  Hydrogen  antimonide. 

Strontium,  Sr. 

Decomp.  by  H2O  with  violence.  Dil. 
H2SO4,  and  HCl+Aq  decomp.  and  dissolve; 
cold  H2SO4  attacks  slowly.  Fuming  HNO3 
has  scarcely  any  action  even  when  boiling. 
(Franz,  J.  pr.  107.  253.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  829.) 

Sol.  in  excess  of  liquid  NH3  at  — 60°  form- 
ing Sr(NH3)6.  (Roederer,  C.  R.  1905,  140. 
1252.) 

Strontium  amalgam,  SrHgi2. 

Stable  below  30°.  Above  30°  the  com- 
position of  the  amalgam  varies.  Can  be 
cryst.  from  Hg  at  any  temp,  below  30°. 
(Kerp,  Z.  anorg.  1900,  25.  68.) 

Strontium  amide,  Sr(NH2)2. 

(Roederer,  Bull.  Soc.  1906,  (3)  36.  715.) 


860 


STRONTIUM  ARSENIDE 


Strontium  arsenide,  Sr3As2. 

Decomp.  by  H2O.     (Lebeau,  C.  R.  1899, 
129.  47.) 

Strontium  azoimide,  SrN6. 

Hydroscopic. 

45.83  pts.  are  sol.  in  100  pts.  H2O  at  16°. 

0.095     "    "     "    "  100    "  abs.  alcohol  at 
16°. 


Strontium  carbide,  SrC2. 

Easily  decomp.  by   H2O   and   dil.  acids. 
(Moissan,  Bull.  Soc.  1894,  (3)  11.  1008.) 

Strontium  carbonyl,  Sr(CO)2. 

(Roederer,  Bull.  Soc.  1906,  (3)  35.  725.) 

Strontium  chloride,  SrCl2,  and  +6H2O. 
Deliquescent  in  moist  air.. 


Insol.  in  pure  etner.    (Uurtms,  J.  pr.  1898, 

Sol.  in  1.5  pts.  HzO  at  15°,  and  0.8  pt.  at  boiling 

(2)  58.  287.) 

(Dumas);  in  1.996  pts.  H2O  at  15°  (Gerlach). 

1  pt.  anhydrous  SrCh  is  sol.  in  2.27  pts.  EUO  at  0°; 

Strontium  boride,  SrB6. 
Sol.  in  fused  oxidizing  agents;  not  decomp. 

in  1.88  pts.  at  20°;  in  1.54  pts.  at  40°;  in  1.18  pts.  at  60°; 
in  1.08  pts.  at  80°;  in  0.98  pt.  at  100°.    (Kremers,  Pogg. 
103.  66.) 

by  H2O;  insol.  in  aq.  acids;  si.  sol.  in  cone. 
H2SO;  sol.  in  dil.  and  cone.  HN03.    (Moissan, 
C.  R.  1897,  125.  633.) 

100  pts.  H2O  dissolve  106.2  pts.  SrCl2-f 
6H2O  at  0°,  and  205.8  pts.  at  40°.    (Tilden, 
Chem.  Soc.  45.  409.) 

Strontium  bromide,  SrBr2,  and  +6H2O. 

100  pts.  H2O  dissolve  at: 

Solubility  in  100  pts.  H2O  at  t° 

0°      20°    38°     59°     83°     110° 

Pts. 

Pts. 

Pts. 

87.7     99      112     133     182    250  pts.  SrBr2. 

t 

SrCl2 

t° 

SrCl2 

t° 

SrCh 

(Kremers,  Pogg.  103.  65.) 

0 

44.2 

41 

67.4 

81 

92.7 

Sat.  SrBr2+Aq  contains  at: 

1 

44.5 

42 

68.2 

82 

93.1 

—11°       —1°       +7°       18° 

2 

44.8 

43 

68.9 

83 

93.4 

43.1        46.85      48.2       51.7%  SrBr2, 

3 

45.2 

44 

69.7 

84 

93.7 

- 

4 

45.6 

45 

70.4 

85 

94.1 

20°          93°         97°       107° 
51.8         68.5       68.7       69.8%  SrBr2. 

5 
6 

46.0 
46.5 

46 

47 

71.2 
72.0 

86 

87 

94.5  . 
94.9 

(fitard,  A.  ch.  1894,  (7-)  2.  540.) 

7 

46.9 

48 

72.8 

88 

95.4 

Sp.  gr.  of  SrBr2+19.5°  containing: 
5           10          15         20          25  %  SrBr2, 
1.046     1.094     1.146     1.204     1.266 

8 
9 
10 
11 

47  .4 

47.8 
48.3 
48.8 

49 
50 
51 
52 

73.6 
74.4 
75.3 
76.1 

89 
90 
91 
92 

95.8 
96.2 
96.7 
97.2 

30         35          40         45          50  %  SrBr2. 

12 

49.4 

53 

77.0 

93 

97.9 

1.332     1.41       1.492     1.59       1.694 

13 

49.9 

54 

77.9 

94 

98.2 

(Kremers,  Pogg.  99.  444;  calculated  by 
Gerlach,  Z.  anal.  8.  285.) 

14 
15 

50.4 
51.0 

55 
56 

78.7 
79.6 

95 
96 

98.8 
99.4 

16 

51.5 

57 

80.4 

97 

100  0 

Somewhat  sol.  in  absolute  alcohol.  (Lowig.) 
Solubility  of  anhydrous  SrBr2  in  alcohol 
is  practically  constant  between  0°  and  40°, 
100  com.  of  abs.  alcohol  dissolving  about  64.5 
g.  of  the  anhydrous  salt  and  forming  a  solu- 

17 
18 
19 
20 
21 

52.1 
52.7 
53.3 
53.9 
54.5 

58 
59 
60 
61 
62 

81^3 
82.2 
83.1 
84.0 
84.9 

98 
99 
100 
101 
102 

103^6 
101.3 
101.9 
102.6 
103.3 

tion  having  a  sp.  gr.  =  1.210  at  0°.    (Fonzes- 

22 

55.1 

63 

85.8  . 

103 

104.0 

Diacon,  Chem.  Soc.  1895,  68  (2)  223.) 
Much  more  sol.  than  BaBr2  in  boiling  amyl 

23 
24 

55.7 
56.3 

64 
65 

86.6 
87.5 

104 
105 

104.7 
105.4 

alcohol. 

25 

56.9 

66 

88.4 

106 

106  1 

Insol.  in  benzonitrile.    (Naumann,  B.  1914, 

26 

57.5 

66.5 

88.8 

107 

106^9 

47.  1370.) 

27 

58.1 

67 

88.9 

108 

107.6 

Difficultly  sol.  in  methyl  acetate.     (Nau- 

28 

58.7 

68 

89.1 

109 

108.4 

mann,  B.  1909,  42.  3790.) 

29 

59.3 

69 

89.3 

110 

109.1 

Strontium  stannic  bromide. 

30 
31 

60.0 
60  6 

70 
71 

89.6 
89.8 

111 
112 

109.9 
130.7 

See  Bromostannate,  strontium. 

32 

6l!3 

72 

113 

111.4 

Strontium  bromide  ammonia,  2SrBr2,  NH3. 

33 

61.9 

73 

90^3 

114 

112.2 

Sol.  in  H2O.    (Rammelsberg,  Pogg.  55.  238. 

34 
35 

62.5 
63.2 

74 
75 

90.6 
90.9 

115 
116 

113.0 
113.8 

Strontium  bromide  hydrazine,  SrBr2,  3N2H4. 

36 

63.9 

76 

91.2 

117 

114.6 

Very  sol.  in  H2O.     (Franzen,   Z.  anorg. 

37 

64.6 

77 

91.5 

118 

115.5 

1908,  60.  290.) 

38 

65.3 

78 

91.8 

118.8 

116.4 

39 

66  0 

70 

Q2   1 

Strontium  bromofluoride,  SrF2,  SrBr2. 

40 

66^7 

i  \y 

80 

"^  .    J. 

92.4 

•    Decomp.  by  H2O.    (Defacqz,  A.  ch.  1904, 

(8)  1.  356.) 

(Mulder,  Scheik.  Verhandel.  1864.  118.) 

STRONTIUM  CHLORIDE 


861 


100  pts.  H2O  dissolve  52.4  pts.  SrCl2  at  18°. 
(Gerardin.) 

Sat.  SrCl2+Aq  contains  %  SrCl2  at  t°. 

Sp.  gr.  of  SrCl2+Aq  at  18°. 

%SrCl2 

Sp.  gr. 

%  SrCh 

Sp.  gr. 

5 
10 
15 

1.0443 
1.0932 
1  .  1456 

20 
22 

1.2023 
1.2259 

t° 

%  SrClj 

t° 

%  SrClz 

-17 
-11 
-   5 
-    1 
+  2 
7 
18 
21.5 
35 
44.5 
54 
55 
59 
64 
70 

26.5 
28.6 
29.3 
30.8 
31.3 
31.7 
33.7 
34.7 
37.8 
39.8 
42.8 
43.8 
47.7 
46.4 
46.1 

75 

80- 
92 
98 
104 
105 
118 
132 
144 
153 
175 
215 
222 
250 

46.5 
47.1 
47.5 
49.6 
50.7 
50.7 
52.0 
52.5 
54.7 
55.7 
60.5 
64.1 
65.4 
67.3 

(Kohlrausch,  W.  Ann.  1879.  1.) 

Sp.  gr.  of  SrCl2+Aq  at  0°.    S=pts.  SrCl2  in 
100  pts.  solution. 

s 

Sp.  gr. 

S 

Sp.  gr. 

31.8193 
27.7170 
23.2300 

1.3609 
1.3086 
1.2515 

18.2629 
12.9997 
6.7243 

1.1915 
1  .  1284 
1.0637 

(Charpy,  A.  ch.  (6)  29.  24.) 

Sat.  SrCl2+Aq  boils  at  114°  (Kremers); 
118.8°  (Mulder);  117.45°,  and  contains  117.5 
pts.  SrCl2  to  100  pts.  H2O  (Legrand)  ;  forms  a 
crust  at  115.5°,  and  contains  120.7  pts.  SrCl2  to 
100  pts.  H2O;  highest  temp,  observed,  119°. 
(Gerlach,  Z.  anal.  26.  436.) 

(fitard,  A  ch.  1894,  (7)  2.  535.) 

SrCh+Aq  sat.  at  8°  has  sp.  gr.  =1.379.    (Anthon,  A. 
24.  211.) 

Sp.  gr.  of  SrCl2+Aq. 


Pts.  SrCh 
to  100  pts.  H2O 

Sp.  gr. 

Pts.  SrC!2 
to  100  pts.  H2O 

Sp.  gr. 

9.81 
20.12 
30.57 

1  .  0823 
1.1632 
1  .  2401 

41.04 
51.69 

1.3114 
1.3816 

(Kremers,  Pogg.  99.  444.) 
Sp.  gr.  of  SrCl2+Aq  at  15°. 


%  SrCl2 

Sp.  gr. 

%  SrCl2 

Sp.  gr. 

5 
10 
15 
20 

1  .  0453 
1.0929 
1  .  1439 
1.1989 

25 

30 
33 

1.2580 
1.3220 
1.3633 

(Gerlach,  Z.  anal.  8.  283.) 


Sp.  gr.  of  SrCl2+Aq   at  24.7°.     a  =  no.  of 
molecules  .  . 
in  grms.  dissolved  in  1,000  g. 

H2O;  b  =  sp.  gr.  when  a  =  SrC!2+6H2O, 
Yz  mol.  SrCl2-|-6H2O  =  133.5  g.;  c  =  sp. 
gr.  when  a  =  Srd2,  1A  mol.  =79.5  g. 


a 

b 

c 

a 

b 

c 

1 

1.063 

1.067 

7 

1.304 

1.401 

2 

1.118 

1.130 

8 

1.330 

3 

1.166 

1.190 

9 

1.354 

. 

4 

1.207 

1.247 

10 

1.376 

.  .  . 

5 

1.243 

1.301 

11 

1.396 

.  .  . 

6 

1.275 

1.352 

(Favre  and  Valson,  C.  R,  79.  968.) 


B.-pt.  of  SrCl2+Aq  containing  pts.  SrCl2  to 
100  pts.  H20.  G  =  according  to  Gerlach 
(Z.  anal.  26.  442);  L  =  according  to  Le- 
grand  (A.  ch.  (2)  69.  436.) 


B.-pt. 

G 

L 

B.-pt. 

G 

L 

101° 

11 

16.7 

110° 

71.4 

68.9 

102 

20.5 

25^.2 

111 

76.5 

74.1 

103 

28.9 

32.1 

112 

81.6 

79.6 

104 

36.2 

37.9 

113 

87 

85.3 

105 

43.2 

43.4 

114 

93.1 

91.2 

106 

49.6 

48.8 

115 

99.5 

97.5 

107 

55.4 

54.0 

116 

105.9 

104.0 

108 

60.8 

59.0 

117 

112.3 

110.9 

109 

66.2 

63.9 

117.5 

.  •  •  • 

Melts  in  its  crystal  H2O  at  112°.     (Tilden, 
Chem.  Soc.  46.  409.) 


Sp.  gr.  of  SrCl2+Aq  at  25°. 


Concentration  of  SrCl2+Aq. 

Sp.  gr. 

1-normal 
Vr-       " 

Vr-       " 
Vr-       " 

1.0676 
1.0336 
1.0171 
1.0084 

(Wagner,  Z.  phys.  Ch.  1890,  6.  40.) 

SrCl2+Aq  containing  3.24%  SrCl2  has  sp. 
gr.  20°/20°  =  1.0284. 

SrCl2+Aq  containing  7.08%  SrCl2  has  sp. 
gr.  20°/20°  =  1.0638. 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896> 
19.  279.) 


862 


STRONTIUM  THALLIC  CHLORIDE 


Sp.  gr.  of  SrCl2+Aq  at  20°. 


g.  mols.  SrCh  per  1. 

Sp.  gr. 

0.01 

.0012284 

0.02937 

.0038396 

0.03987 

.0053832 

0.05017 

.007028 

0.07077 

.009560 

0.10 

.013205 

0.25 

- 

.034433 

0.50 

.068379 

0.75 

.  101760 

1.00 

.  135423 

(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38.  697.) 

Cone.  HCl+Aq  ppts.  part  of  the  SrCl2 
from  SrCl2+Aq.    (Hope.) 

Solubility  of  SrCl2  in  HCl  +  Aq  at  0°.  SrCl2  = 
Y^  mols.  SrCl2  (in  milligrammes)  dis- 
solved in  10  ccm.  of  liquid;  HCl  =  mols. 
HC1  (in  milligrammes)  dissolved  in 
10  ccm.  of  liquid. 


SrCh 

HCl 

Sum  of  mols. 

Sp.  gr. 

55 

48.2 
41.25 
30.6 

0 
6.1 
12.75 
23.3 

55.0 
54.3 
54.00 
53.9 

1.334 
1  .  3045 
1.2695 
1.220 

(Engel,  Bull.  Soc.  (2)  45.  655.) 
Solubility  of  SrCl2  in  HCl+Aq  at  0°. 


Mg.  mols.  per  10  cc. 
solution 

Sp.  gr.  of 
solution 

G.  per  100  cc. 
solution 

SrCh 
2 

HCl 

SrCl* 

HCl 

51.6 
44.8 
37.85 
27.2 
22.0 
14.0 
4.25 

0 
6.1 
12.75 
23.3 

28.38 
37.25 
52.75 

.334 
.304 
.269 
.220 
.201 
.167 
.133 

40.9 
35.5 
30.0 
21.56 
17.44 
11.09 
3.37 

0.0 
2.22 
4.65 
8.49 
10.35 
13.58 
19.23 

(Engel,  A.  ch.  1888,  (6)  13.  376.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch.  J. 
1898,  20.  829.) 

Sol.  in  6  pts.  alcohol  of  0.833  sp.  gr.  at  15°.  (Vau- 
quelin.) 

Sol.  in  24  pts.  absolute  alcohol  at  15°.  and  in  19  pts.  at 
boiling.  (Bucholz.)  Sol.  in  2.5  pts.  of  boiling  alcohol. 

Anhydrous  SrCl2  is  sol.  in  111.6-116.4  pts. 
alcohol  of  99.3%  at  14.5°,  and  in  26.2  pts.  of 
the  same  alcohol  at  boiling.  (Fresenius,  A. 
69.  127.) 

100  pts.  alcohol  of  given  sp.  gr.  at  0°  dis- 
solve pts.  SrCl2  at  18°. 
0.990    0.985    0.973    0.966    0.953  sp.  gr. 
49.81     47.0       39.6      35.9      30.4  pts.  SrCl2, 


0.939 
26.8 


0.909 
19.2 


0.846 
4.9 


0.832  sp.  gr. 
3.2  pts.  SrCl2. 


Insol.  in  absolute  alcohol.  (Gerardin,  A. 
ch.  (4)  6.  156.) 

100  pts.  absolute  methyl  alcohol  dissolve 
63.3  pts.  SrCl2+6H2O  at  6°;  ethyl  alcohol, 
3.8  pts.  (de  Bruyn,  Z.  phys.  Ch.  10.  787.) 

SI.  sol.  in  boiling  amyl  alcohol.  (Browning, 
Sill.  Am.  J.  144.  459.) 

100  g.  95%  formic  acid  dissolve  23.8  g.  SrCl2 
at  room  temp*.  (Aschan,  Ch.  Ztg.  1913,  37. 
1117.) 

Absolutely  insol.  in  acetic  ether.  (Cann, 
C.  R.  102.  363.) 

Very  si.  sol.  in  acetone.  (Krug  and 
M'Elroy.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014.) 

Insol.  in  methyl  acetate.     (Naumann,  B. 

1909,  42.  3790.) 

Insol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1370.) 

SI.  sol.  in  anhydrous  pyridine.  Sol.  in 
97%,  95%  and  93%  pyridine +Aq.  (Kahlen- 
berg,  J.  Am.  Chem.  Soc.  1908,  30.  1107.) 

+2H2O.  Tr.  pt.  from  +6H2O  is  61.5°. 
(Richards  and  Churchill,  Z.  phys.  Ch.  1899, 
28.  313.) 

+6H2O.    See  above. 

Strontium  thallic  chloride,   SrCl2,   2T1C13  + 

6H2O. 
(Gewecke,  A.  1909,  366.  223.) 

Strontium    tin    (stannous)    chloride,    SrCl2, 
SnCl2+4H2O. 

Sol.  in  H2O.    (Poggiale,  C.  R.  20.  1183.) 
Strontium  tin  (stannic)  chloride. 

See  Chlorostannate,  strontium. 
Strontium  uranium  chloride,  SrCl2,  UC14. 

Decomp.  by  H2O.     (Aloy,  Bull.  Soc.  1899, 
(3)  21.  265.) 
Strontium  zinc  chloride,  SrZnCl4+4H2O. 

Very  sol.  in  H2O.     (Ephraim,  Z.   anorg. 

1910,  67.  380.) 

Strontium  chloride  ammonia,  SrCl2,  8NH3. 
Decomp.  by  H2O.    (Rose,  Pogg.  20.  155.) 

Strontium  chloride   hydrazine,  SrCl2,  2N2H4 

+H20. 

Hydroscopic.      (Franzen,   Z.   anorg.    1908, 
60.  289.) 
Strontium   chloride   hydroxylamine,   2SrCl2, 

5NH2OH+2H2O. 

As  Ca  comp.     (Antonow,  J.  Russ.  Phys. 
Chem.  Soc.  1905,  37.  482.) 
Strontium  hydrogen  chloride  hydroxylamine, 

2SrCl2,  3HC1,  9NH2OH+H2O. 
(Antonow,  J.  Russ.  Phys.  Chem.  Soc.  1905, 
37.  482.) 
Strontium  chlorofluoride,  SrF2,  SrCl2. 

Decomp.  by  H2O,  by  very  dil.  HCl,  HNO3 
or  acetic  acid,  by  hot  dil.  or  cone.  H2SO4. 


STRONTIUM  HYDROXIDE 


863 


Sol. 

in  cone.  HC1  or  HNO3.    Insol.  in,  and 

1                                                1                                 It                               1            -1  •                              Ill 

Solubility  in  Sr(NX)3)2+Aq  at  25°. 

not 

decom 

p.    oy    co 

id    or 

Donmg 

aiconoi. 

Sp.  gr.  25°/25° 

G.  SrO  as 
Sr(OH)2in 
100  g.  H2O 

(Defacqz,  A.  ch.  1904 

,(8)1 

.  355.) 

G.  Sr(NO3)2in 
100  g.  H2O 

Strontium  fluoride,  SrF2. 

Somewhat  sol.  in  H2O.    (Fr.  Roder.) 

1.481 

0. 

0 

79.27 

1] 

.H2O 

dissolves  113.5  mg.  SrF2 

at  0.26°; 

* 

1.506 

1. 

76 

81.06 

117.3    mg. 

at   17.4°: 

119.3    mg. 

at    27.4°. 

1.490 

1. 

71 

74.27 

(Kohlrausch,  Z.  phys 

Ch.  1908,  64 

168.) 

1.450 

1. 

55 

66.88 

Insol  in  HF+Aq. 

(Berzelius.) 

1.419 

1. 

51 

63.71 

Boiling  HCl+Aq  dissolves;  si.  attacked  by 

1.403 

1. 

47 

60.37 

boiling  HNO3+Aq;  decomp.  by  hot  H2SO4. 

1.381 

1. 

41 

56.30 

(Poulenc,  C.  R.  116.  987.) 

1.359 

1. 

34 

52.90 

1.327 

1. 

27 

46.97 

Strontium  stannic  fluoride. 

l!317 

1. 

20 

44^03 

See  Fluostannate,  strontium. 

1.291 

1. 

14 

40.83 

Strontium  titanium  fluoride. 

1.267 
1.239 

1.11 

1.02 

37.81 
32.41 

See  Fluotitanate,  strontium. 

1.217 

i! 

01 

28^80 

Strontium  fluoiodide, 

SrF2. 

SrI2. 

1.206 

0. 

96 

26.58 

Decomp.  by  cold  H2O,  more  rapidly  by  hot 
H2O.    Decomp.  by  dil.  HC1,  dil.  HNO3,  dil. 
H2SO4  or  cone.  H2SO4,  also  by  alcohol  and  by 
ether,  if  not  absolute.    (Defacqz,  A.  ch.  1904, 

/O\    4        O  PT>     \ 

1.178 
1.148 
1.126 
1.108 
1.079 

00000 

95 
91 

87 
84 
81 

23.83 
17.96 
16.21 
12.78 
8.96 

(8)  1 

ooo.; 

1.059 

0. 

79 

6.29 

Strontium  hydride,  SrH. 

1.033 

0. 

78 

4.45 

Decomp. 
B.  24.  1976 

oy  ±12U  or  JHJi-1-Aq.  . 

(Winkler, 

*Solution  is  sat.  with  respect  to  both  sub- 

SrH2.   Decomp.  by 
1902,  134.  100.) 

H2O. 

(Gautier,  C.  R. 

stances. 
(Parsons  and  Perkins,  J.  Am.  Chem.  Soc. 

Strontium  hydroselenide. 

1910,  32.  1388.) 

Sol.  in  H2O. 

Sol.  in  methyl  alcohol 

At  room  temp.  1 

Strontium  hydrosulphide,  SrS2H2. 
Sol.  in  H2O;  decomp.  by  boiling. 

1.  contains  31.5  g.  SrO.     (Neuberg  and  Re- 
wald,  Biochem.  Z.  1908,  9.  540.) 
Insol.  in  acetone.     (Eidmann.  C.  C.  1899. 

Strontium  hydroxide, 

SrO2H2,  and  +8H2O. 

II.  1014.) 

Deliquescent. 

Sol.  in  an  aqueous  solution  of  cane  sugar. 

Sol. 

in  50  pts.  cold,  and  2.4  pts.  boiling  H2O  (Bu- 

(Hunton,  Phil.  Mag.  (3) 

11.  156.) 

cholz) 

:  in  50  i 

5ts.  H2O  at 

15.56° 

Dalton)  ; 

in  51.4  nts. 

H2O  at  15.56°,  and  2  pts.  at  100°  (Hope)  ;  in  52  pts.  H2O 
at  15°,  and  2.4  pts.  at  100°  (Berzelius)  ;  in  48  pts.  H2O 

j.     1  O    TCO     /  A  Ul\ 

Solubility  in  H2O  containing  10  g.  sugar  at  t°. 

at  18.75"  (AM). 
100  pts.  H2O  at  20°  dissolve  1.49  pts.  SrO.     (Bineau, 

t° 

g.  SrO2H2+8H2O 

t°        g.  SrO2H2+8H2O 

C.  R. 

A  1     AOQ 

100  pts.  aqueous  solution  of  SrO2H2  contain 

3 

3.10 

24              4.79 

pts.  SrO 

and  pts.  SrO2H 

2-f8H2O  at  t°. 

15 

3.79 

40              9  .  70 

Pts. 

^  Pts. 

Pts. 

Pts. 

(Sidersky,  C. 

C 

1886.  57.) 

t° 

SrO 

+8H2O 

t° 

SrO 

SrO2H2 
+8H2O 

_i_, 

^TToO      0  083*5  mn 

i  i 

a    ortl      ir.    1     1      TT.n    o* 

0 

0.35 

0.90 

55 

2.54 

6.52 

T^< 

25°. 

3-Ll2V/»       vs.vsOOO   IllOx.    10   OWA,   AH    J.    i.    J-JL^V^    c^u 

(Rothmund,  Z.  phys.  Ch.  1909,  69.  539.) 

5 

0.41 

1.05 

60 

3.03 

7.77 

10 
15 

0.48 
0  57 

1.23 
1  46 

65 
70 

3.62 
4.35 

9.29 
11  16 

Solubility  in  organic 

compds.  +Aq  at  25°. 

20 

0.68 

1.74 

75 

5.30 

13^60 

Solvent 

Mol.  SrO2H2+8H2O 

25 

0.82 

2.10 

80 

6.56 

16.83 

sol.  in  llitre 

30 

1.00 

2.57 

85 

9.00 

23.09 

35 
40 
45 
50 

1.22 
1.48 
1.78 
2.13 

3.13 
3.80 
4.57 
5.46 

90 
95 
100 

12.00 
15.15 
18.60 

30.78 

38.86 
47.71 

water 
0  .  5-N  methyl  alcohol 
ethyl  alcohol 
propyl  alcohol 

0.0835 
0.0820 
0.0744 
0.0708 

. 

tert.  amyl  alcohol 

0.0630 

(Scheibler,  J.  pharm.  China. 

1883,  (5)  8.  540.) 

acetone 

0.0692 

Sol.  in  cold  NH4Cl+Aq. 

(Rose.) 

ether 

0.0645 

864 


STRONTIUM  IODIDE 


Solubility  in  organic  compds.+Aq  at  25°. — 
Continued. 


Solvent 


0.5-N  glycol 

glycerine 

mannitol 

urea 

ammonia 

diethyl  amine 

pyridine 


Mol.  SrO2H2+8H2O 
sol.  id  1  litre 


0.0922 

0.1094 
0.1996 
0.0820 
0.0785 
0.0586 
0.0694 


(Rothmund,  Z.  phys.  Ch.  1909,  69.  539.) 

Insol.  in  acetone.    (Naumann,  B.  1904,  37. 
4329.) 
See  also  Strontium  oxide. 

Strontium  iodide,  SrI2j  and  +6,  or  7H2O. 
100  pts.  H2O  dissolve  at: 
0°     20°     40°     70°     100° 
164     179     196    250     370  pts.  SrI2. 
(Kremers,  Pogg.  103.  65.) 

Sat.  aq.  solution  contains  at: 
—20°  —10°  —3°  +7°    11°     18°  38° 
60.0     60.3    62.2  63.0  63.4  63.5  64.8%  SrI2, 

52°   63°   77°   81°    97°    105°  120 175° 
66.0  68.5  70.5  74.0  79.2  79.4  80.8  85.6%  SrI2. 
(Etard,  A.  ch.  1894,  (7)  2.  543.) 

Sp.  gr.  of  SrI2+Aq  at  19.5°  containing: 

5  10         20         30  %  SrI2; 

1.045     1.091     1.200     1.330 

40         50         60         65  %  SrI2. 
1.491     1.695     1.955     2.150 
(Kremers,  Pogg.  103.  67;  calculated  by 
Gerlach,  Z.  anal.  8.  285.) 

Sat.  solution  in  abs.  ethyl  alcohol  contains 
at: 

—20°       +4°      39°      82° 
2.6          3.1        4.3       4.7%SrI2. 
(Etard,  A.  ch.  1894,  (7)  2.  565.) 

Strontium  periodide,  SrI3  +  15H2O. 
(Mosnier,  A.  ch.  1897,  (7)  12.  399.) 
SrI4.    (Herz  and  Bulla,  Z.  anorg.  1911,  71. 

255.) 

Strontium  stannous  iodide. 
Very  sol.  in  H2O.    (Boullay.) 

Strontium  zinc  iodide,  SrZnI4+9H2O. 

Hydroscopic.     (Ephraim,  Z.  anorg.  1910, 
67.  385.) 

Strontium  nitride,  Sr2N3. 

Decomp.  H2O  violently,  but  not  alcohol. 
(Maquenne,  A.  ch.  (6)  29.  225.)    , 


Strontium  oxide,  SrO. 

Decomp.  by  H2O  to  SrO2H2,  which  see. 

Sol.  in  160  pts.  H2O  at  15.56°  (Dalton) ;  in  50  pts.  at 
100°  (Dalton) ;  in  130  pts.  at  20°  (Bineau) ;  in  40  pts. 
cold,  and  20  pts.  hot  H2O  (Dumas). 

Very  si.  sol.  in  alcohol.    Insol.  in  ether. 

1  1.  methyl  alcohol  dissolves  11.2  g.  SrO. 
(Neuberg  and  Rewald,  Biochem.  Z.  1908,  9. 
540.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Sol.  in  cane  sugar +Aq. 

Solubility  in  H2O  containing  10  g.  sugar  at  t°. 


8 
15 


g.  SrO 


1.21 

1.48 


24 
40 


g.  SrO 


1.87 
3.55 


(Sidersky,  C.  C.  1886.  57.) 
See  also  Strontium  hydroxide. 

Strontium  peroxide,  SrO2. 

SI.  sol.  in  H2O.  Easily  sol.  in  acids  and 
NH4Cl+Aq.  Insol.  in  NH4OH+Aq.  (Con- 
roy,  Chem.  Soc.  (2)  11.  812.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Strontium  oxybromide,  SrBr2,  SrO+9H2O. 

Not  hydroscopic;  sol.  in  H20.  (Tassilly, 
C.  R.  1895,  120.  1339.) 

Strontium  oxychloride,  SrCl2,  SrO+9H2O. 

Very  easily  decomp.  by  H2O  and  alcohol. 
(Andre*,  A.  ch.  (6)  3.  76.) 

Strontium  oxyiodide,  2SrI2,  5SrO+30H2O. 

Not  hydroscopic;  sol.  in  H2O.  (Tassilly, 
C.  R.  1895,  120.  1339.) 

Strontium  oxysulphide,  Sr2OS4  +  12H2O. 
Decomp.  by  H2O. 

Insol.  in  alcohol,  ether,  and  CS2.    (Schone.) 
Mixture  of  SrS2O3  and  SrS2.    (Geuther,  A. 

224.  178.) 

Strontium  phosphide,  Sr3P2. 

Crystallized.  Sol.  in  dil.  acids;  insol.  in 
cone,  acids;  decomp.  by  H2O.  Insol.  in  or- 
ganic solvents  at  ord.  temp.  (Jaboin,  C.  R. 
1899,  129.  764.) 

Strontium  selenide,  SrSe. 

SI.  sol.  in  H2O.    (Fabre,  C.  R.  102.  1469.) 

Strontium  silicide,  SrSi2. 

Decomp.  by  H2O.  (Bradley,  C.  N.  1900, 
82.  150.) 


SULPHANTIMONATES 


865 


Strontium  sulphide,  SrS. 

Sol.  in  H2O  with  decomp.  into  SrO2H2  and 
SrS2H2. 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 

Insol.  in  methyl  acetate.  (Naumann,  B 
1909,  42.  3790.) 

Strontium  tetrasulphide,  SrS4. 

Very  deliquescent,  and  sol.  in  H2O  anc 
alcohol.  Aqueous  solution  decomp.  on  air 
Cryst.  with  2,  or  6H2O.  (Schone,  Pogg.  117, 

58.) 

Strontium  pentasulphide,  SrS5. 
Known  only  in  solution. 

Strontium  stannic  sulphide. 
See  Sulphostannate,  strontium. 

Sulphaluminic  acid. 

Silver  sulphaluminate,  4Ag2S,  5A12S?. 

(Cambi,  Real.  Ac.  Line.  1912,  (5)  21,  II. 

837.) 

Sulphamic  acid,  HOS02NH2. 
See  Amidosulphonic  acid. 

Ammonium  sulphamate,  2NH3,  SO3. 

(Woronin.) 

Is  ammonium  imidosulphonate,  which  see. 
(Berglund.) 

Ammonium  sulphamate,  acid,  3NH3,  2SO3. 

(Woronin.) 

Is  basic  ammonium  imidosulphonate,  which 
see.  (Berglund.) 

Barium  sulphamate,  basic,  2BaO,  3SO3,  2NH3 
Somewhat  sol.  in  H2O,  easily  in  HCl+Aq. 

(Jacquelain,  A.  ch.  (3)  8.  304.) 
BaS2O6(NH2)2.    SI.  sol.  in  H2O.    Decomp. 

by  heating  with  H2O.     (Woronin,  J.  B.  1860. 

80.) 

Is  barium  imidosulphonate.    (Berglund.) 

Sulphamide,  SO2(NH2)2. 

Very  sol.  in  H2O.  (Regnault,  A.  ch.  69. 
170;  Mente,  A.  248.  267.) 

Insol.  in  alcohol,  ether,  etc.  (Traube,  B. 
26.  607.) 

Very  sol.  in  H2O. 

SI.  sol.  in  abs.  alcohol. 

SI.  sol.  in  dry  ether.  (Divers  and  Ogawa, 
Chem.  Soc.  1902,  81.  504.) 

Very  sol.  in  liquid  NH3.  (Franklin  and 
Stafford,  Am.  Ch.  J.  1902,  28.  95.) 

Sol.  in  alcohol;  very  sol.  in  H2O.  (Hantzsch, 
B.  1901,  34.  3436.) 


Silver  sulphamide,  SO2(NHAg)2. 

SI.  sol.  in  cold  H2O.  Sol.  in  HNO3,  and 
(NH4)2CO3+Aq.  (Traube,  B.  26.  607.) 

3NH3,  2SO3.     (Jacquelain.) 

Is  basic  ammonium  imidosulphonate,  which 
see.  (Berglund.) 

Sulphamidic  acid. 

(Fremy.) 

See  Imidosulphom'c  acid. 

Sulphaminoplatinous  acid. 

Ammonium  tefrasulphaminoplatinite. 

[Pt(SO3NH2)4](NH4)2+6H2O. 
SI.  sol.  in  cold  H2O.    (Ramberg,  B.  1912, 
46.  1512.) 

Potassium ,  [Pt(SO3NH2)4]K2+2H2O. 

Very  si.  sol.  in  cold  H2O.     (Ramberg.) 

Sodium . 

Easily  sol.  in  cold  K^O.     (Ramberg.) 

Sulphammonic,  and  Metasulphammonic 
acids. 

(Fremy.) 

See  Nitrilosulphonic  acid. 

Mowosulphammonic  acid. 
(Glaus.) 
See  Amidosulphonic  acid. 

ZH'sulphammonic  acid. 

(Glaus.) 

See  Imidosulphonic  acid. 

Tn'sulphammonic  acid. 

(Glaus.) 

See  Nitrilosulphonic  acid. 

Tetrasulphamm  onic  acid. 

(Glaus.) 

Does  not  exist.    See  Nitrilosulphonic  acid. 

Sulphammonium,  S(NH3)2,  2NH3. 
Sol.  in  liquid  NH3. 

Sol.  in  abs.  alcohol  and  anhydrous  ether. 
Moissan,  C.  R.  1901,  132.  517.) 

Sulphantimonic  acid. 

Sulphantimonates. 
The  alkali  sulphantimorrates  are  sol.   in 

I2O,  but  the  solutions  decomp.  on  the  air; 
most  of  the  other  sulphantimonates  are  insol. 

n  H2O;  all  sulphantimonates  are  insol.  in 
alcohol.    (Rammelsberg.) 


866 


SULPHANTIMONATE,  AMMONIUM 


Ammonium  sulphantimonate,  (NH4)3SbS4. 

Sol.  in  H?O. 

Sol.  in  dil.  acids  with  decomp.     (Stanek, 
Z.  anorg.  1898.  17.  122.) 

+4H2O.    (Stanek.) 

Solubility  of  (NH4)3SbS4+4H2O  in  H2O  at  t°. 


Iron    (ferric)    sulphantimonate,    Fe2(SbS4)2. 
(Rammelsberg,  Pogg.  62.  234.) 

Lead  sulphantimonate,  Pb3(SbS4)2. 

Ppt.    Decomp.  by  KOH+Aq.    (Rammels- 
berg, Pogg.  62.  223.) 


*o                         % 

*    .         (NH4)3SbS4 

Solid  phase 

Lithium  sulphantimonate,  Li3SbS4+8^2H2O. 
100  g.  sat.  solution  in  H2O  contain  50.8  g. 

-  1.9          9.9 

Ice 

anhyd.  Li3SbS4. 

-  5            20.0 
—  8            30  2 

(( 

Solubility  in  alcohol  at  30°. 

-13.5        41.6 
0            41.6 

Ice+(NH4)3SbS4,  4H2O 
(NH4)3SbS4,  4H2O 

** 

alcohol 

Li3SbS4 

Solid  phase 

+20            47  .  7 

30            54.5 

ii 

0 

50.8 

Li»SbS4,  8^H2O 

13.3 

46.3 

u 

(Donk,  Chem.  Weekbl,  1908,  5.  529.) 

51.9 

30.7 

tl 

54.8 

29.9 

11 

Solubility  of  (NH4)3SbS4  in  alcohol  at  10°. 

58.4 

KO     f\ 

30.8 

qo    q 

T  '    C*1^O       Ol  /TJT   /^V    1    T  "    w'  I    >*J 

ljl3ODio4.  O7/2rl2vJ-p-Lil3ODia4 

tt 

Solid  phase,  (NH4)3SbS4+4H2O. 

Oo  .  O 

65.26 

o£  .  o 

29.31 

LisSbS4 

cr                        07 

07 

gf 

74.3 

24.1 

a 

C2H6OH       (NH4)3SbS4        C2H8OH 

'(NH4)°3SbS4 

79.5 

20.5 

" 

0                43.2 

43.1 

8.7 

(Schreinemakers   and   Jacobs,    Ch.    Weekbl. 

5.1            35.9 

53.1 

4.1 

1910,  72.  213.) 

19.1            23.1 

93.3 

0 

I    rvTT    S^i            T7"                         1        *          TT    /~\            /T>      *      1 

(Donk,  I.  c.) 

+9H2O.    Very  sol.  in  H2O.     (Bnnkmann, 
Dissert.  1891.) 

Antimonyl  sulphantimonate,  (SbO)3SbS4. 
Sol.  in  HC1.     (Rammelsberg,  Pogg.  1841, 

+10H2O.     Solubility  of  Li3SbS4+10H2O  in 
H2O  at  t°. 

62.  236.) 

v7 

t° 

Solid  phase 

Barium  sulphantimonate,  Ba3(SbS4)  +3H2O. 

13        L  4 

Sol.  in  H2O.    Insol.  in  alcohol. 

-  1.7 

7.1 

Ice 

-  3.2 

12.8 

(l 

Barium   potassium 

sulphantimonate  , 

-  5.1 

17.5 

lt 

KBaSbS4+6H2O. 

-10.8 

23.2 

11 

Easily  sol.  in  H2O. 
Decomp.   by   acids.      (Glatzel, 
1911,  72.  100.) 

Z.   anorg. 

-15.9 
-26.2 

-42 
0 

28.5 
35.3 
40.4 
45.5 

a 

Ice+Li3SbS4,  10H2O 
Li3SbS4,  10H2O 

Bismuth  sulphantimonate. 

+10 
30 

46.9 
50.1 

ft 

Ppt. 

50 

51.3 

lt 

Cadmium   sulphantimonate. 

Ppt.     (Rammelsberg,  Pogg.  52.  236.) 

Calcium  sulphantimonate,  Ca3(SbS4)2. 
Partially  sol.  in  H2O.    Insol.  in  alcohol. 

Cobaltous  sulphantimonate,  Co3(SbS4)2. 

Ppt.    Decomp.  by  HCl+Aq.     (Rammels- 
berg, Pogg.  62.  236.) 

'Cupric  sulphantimonate,  Cu3(SbS4)2. 
Ppt.     (Rammelsberg,  Pogg.  62.  226.) 

Iron  (ferrous)   sulphantimonate. 
Ppt. 


(Donk,  Chem.  Weekbl.  1908,  5.  629.) 

At  10°,  100  g.  sat.  Li3SbS4+10H2O  in  10.7 
%  alcohol  contain  41.8  g.  Li3SbS4;  26.2% 
alcohol,  36.5  g.  Li3SbS4.  (Donk,  L  c.) 

Magnesium  sulphantimonate,  Mg3(SbO4)2. 

Deliquescent.  Sol.  in  H2O.  Decomp.  by 
alcohol. 

Mercurous  sulphantimonate,  (Hg2)3(SbS4)2. 
Ppt. 

Mercuric  sulphantimonate,  Hg3(SbS4)2. 
Ppt.    (Rammelsberg,  Pogg.  62.  229.) 


SULPHANTIMONATE,  SODIUM 


Mercuric   sulphantimonate   chloride, 

Hg3(SbS4)2,   3HgCl2,   3HgO. 
Insol.  in  acids,  except  aqua  regia.     (Ram- 
melsberg.) 

Nickel  sulphantimonate,  Ni3(SbS4)2. 
Ppt.     Decomp.  by  hot  HCl+Aq.     (Ram- 
melsberg,  Pogg.  52.  226.) 

Potassium  sulphantimonate,  K3SbS4. 
Sol.  in  H2O. 

Solubility  of  KRSbS4  in  H2O  at  t°. 

Composition  of  the  liquid  layers. 

Alcohol  layer                               H2O 

layer 

°7                    °7                    °7 
C2H5OH           K3SbS4             alco°hol 

KaSbS* 

85                  0                  1.1 
54.7              2.2              3.4 
46.9              4.2              3.8 
16                27.4             
31.1 

67.4 
49.0 
45.6 

12.'7 

(Donk,  I.  c.) 

+4V2H2O.     Deliquescent.    Sol.    in    H2O; 
more  sol.  than  the  Na  salt. 
+3,  5,  and  6H2O.     See  Donk  above. 
2K2S,    Sb2S3.      Decomp.    by    cold    H2O. 
(Ditte,  C.  R.  102.  168.) 
K2S,   2Sb2S3+3H2O.     SI.    sol.    in    H2O. 
(Ditte.) 
K2S,  Sb2S3.     Decomp.  by  H2O.     (Ditte.) 
K2S,  2Sb2S3.    (Ditte.) 

Silver  sulphantimonate,  Ag3SbS4. 
Insol.  in  H2O  or  acids.    Decomp.  by  KOH 
+Aq.     (Rammelsberg,  Pogg.  52.  218.) 

Sodium  sulphantimonate,  Na3SbS4+9H2O. 
(Schlippe's  salt.}     Sol.  in  2.9  pts.  H2O  at 
15°.     Aqueous   solution   is   precipitated   by 
alcohol.    (Rammelsberg.) 
Sol.  in  3  pts.  cold  H2O.    (van  den  Corput.) 
Sol.  in  4  pts.  cold  H2O.    (Duflos.) 
Sol.  in  1  pt.  boiling  H2O.    (Duflos.) 

Solubility  of  Na3SbS4+9H2O  in  H2O  at  t°. 

t° 

% 

K  3SbS4 

Solid  phase 

-  1.3 
-  2.6 

-  4 
-  7.2 
-10.6 
-13.5 
-18.5 
-28.8 
-34 
-10 
-  4.5 
0 
+10 
30 
50 
80 

9.5 
17.1 
24.2 
35.4 
42.9 
48.8 
52.6 
59.6 
62 
65.5 
69.1 
75.4 
76.2 
77.1 
77.7 
79.2 

Ice 

H 

(I 

u 
i( 
11 

Ice+K3SbS4,  6H2O 
K3SbS4,  6H2O 

u 

K3SbS4,  5H2O 

u 
u 

K3SbS4,  3H2O 

u 

(Donk,  Chem.  Weekbl.  1908,  5.  529,  629,  767.) 
Solubility  of  K3SbS4  in  KOH+Aq  at  25°. 

% 

KsSbS4 

'     % 

KOH 

Solid  phase 

75 

68.4 
56.8 
50.9 
37.7 
19.8 
11.5 
9.4 
00.0 

0 

3.4 
11.0 
16.1 
25.5 
40.5 
46.9 
49.9 
56.3 

K3SbS4,  5H2O 
K3SbS4,  3H2O 

u 

K3SbS4 

u 

K3SbS4+KOH,  2H20     - 
KOH,  2H2O 

t0             NalbS, 

Solid  phase 

-  0.1           0.5 
-  0.65         4 
-  0.9           5.7 
-  1.26         7.8 
—  1.45         9.2 
-   1.75        11.2 
0             11.3 
15             19.3 
30             27.1 
38             32 
49.6         38.9 
59.6         45 
'  69.6         50.7 
79.5         57.1 

Ice 

H 

U 

tt 

(( 
u 

Na3SbS4,  9H2O 
tt 

u 

n 

<< 
tt 
tt 
tt 

(Donk.) 
Solubility  of  K3SbS4  in  alcohoI+Aq  at  10°. 

% 

C2H53H 

K3SbS4 

Solid  phase 

94 
90.5 

0.8* 
0 

0 
0 

69^2 
76.1 

K3SbS4,  5H2O 

u 
u 

(Donk,  Chem.  Weekbl.  1908,  6.  529 

,  629,  767.) 

*  Two  liquid  layers  are  formed. 

SrU'HANTIMO.VVII.  THIOSI  I. I'll  Ml,    ^>I)|I   \1 


».*« 


Holfd 


Solubility  of  NatSbS4  in  methyl  alcohol  at  t°. 

S.ll.i   |,l,:,   <  . 


.•  -  !..• 


II    S 

1  '1 

o  s 

0    1 

0.0 


0 
4.0 

11   0 

27  3 

:u  (;. 


OH.O 


6H,0 


r  -:<<r 


10.0 
12.5 
4.2 

l 
0 

7.7 
Hi  4 
:*7  7 

47  X 

Nb£bs4,!)H,o 

N 

« 
H 
N 

N\-.,Vb84+Naf8rf)i.4bD 
Na«S*0,,  5H,0 

(Donk,  I.  c.) 

s,liil,iliiy  <»f  >  H.SIKS4  in  aleohol+Aq  at  t°. 
s.h.1  phase,  Na«8b84+OH20. 


t-O* 


0 

a.  7 

12  7 
20. 

.,(1    S 


II  s 

s,i 

(i  D 
0 


t-30* 


5 

10  :i 
21  s 
46 
76.2 


14.6 

(i   4 

i  a 

o 


3 


0 

4.7 
8 

*54.1 
g] 


47.0 


4.1 

0 


*  Two  layers  m 


Composition  of  above  layers. 


Alcohol  layer 

HiO  Uyrr 

%  dflohol 

%  N»«si»S4 

',    :,!<•.  ,!,<.! 

%  Na»8bS4 

54.1 

10  4 

33.5 

4.1 
10  I 

14.1 

8.0 

14  :•; 
18.8 
27.2 

36.5 

27.  s 
24.1 
18.0 

(l)onk,  /.  r.) 


.    !        .1! 


:',  1 

i:,  r, 

2ii  I 

:,o  :', 
57 

81.7 
02 


d  'OH 


H  «i 

2  H 
2    1 

o  :< 
o  i 
o  o:, 
o  2 
2.0 


0 

IX    I 

:<:',  i 

<M     7 

si  2 

HI    2 
!M 


N 


27.1 

12  S 

r,  s 
0.1 
0.1 
1.2 
3.0 


fDonk,  i.  c.) 
Sodium  tulphantimonate  thiosulphate, 


Efflorescent,  and  decomp.  by  H8O.    (lin- 
ger, Arch.  Pharm.  (2)  147.  103.) 
No  double  salt  exists.   See  Donk,  Na^bS4 

undr-r  \:i,SI>S<. 


,1.    in 
I  Ac,; 


Strontium  sulphantimonate. 
Sol.  in  H8O;  pptd.  by 

Uranium  sulphantimonate. 
Ppt. 

Zinc  sulphantimonate,  ZnjfSbS^j. 
Ppt.    Sol.  in  hot  Na«SbS4+Ao: 
Zn8O4-f  Aq.     Partially  sol.  in  KC 
sol.  in  hot  HCl+Aq.    (Rammelsbei 
62.  2 

Sulphantimonous  acid. 


Ammonium  /////</sulphantiim>nitc,  \H4SbSa. 

In.M.i.  n,  n,o.  Houget,  C.  R.  1808,  126. 
1145.) 

+2H|O.    Insol.  in  H2O  and  alcoh-.I. 

Decomp.  in  the  air.  (8tand<,  X.  anorg. 
is!»s,  17.  110.) 

Ammonium  or//?osulphantimonite. 


decomp.  Sl:.l,lc  only  in 
of  (NH4)jS.  SoL  in  H,0.  Insol.  in  alcohol, 
by  which  it  is  pptd.  from  aqueous  solution. 
,  A.  ch.  1800,  (7)  18.  536.) 


Ammonium 


mn/sulphantimonite, 

Sh4S7. 


Stable  in  the  air. 

Insol.  in  H,0. 

Decomp.  by  acids.     (Stanek,   Z.   anorg. 
1808,  17.  120.) 

Stable;  cryst.  from  hot  solutions. 
C.  R.  1808,  126.  1145.) 


Ammonium    silver   ^'/.osuJphamimonite, 
Decamp,  by  HA    (Pouget,  A,  ch,  1899, 


+4V.HA 

JkttoL  in  HA     (Pouget,  A,  eh.   1899, 
(7)11,  ML) 


+8HA 

Decomp,  in  the  air  and  by  HA    Son* 
what  soL  in  BaS+Aq,    (Pouget,  C,  R,  1808, 


i  ////rvfulphantimofiite, 

8Hj0, 
Decamp,  by  HA 
Nearly  insol.  in  BaS+Aq,    (Rouget.) 


Barium  sulphantimonite, 

Pptd.  from  aq.  solution  of  ortho  and  pyro- 
barium  salts    (rouget  ) 

B*8bA,+l«HA    (Pouget,  A,  ch,  1899, 

(7)19,538,) 


Calcium  sulpfaantimonite  bane,  Ca(OH)8bS,, 

In»oL  in  H«O, 

8oL  in  cone,  HCL    (Pouget,  A,  ch,  1899, 
(7)10,544.) 


Calcium  ^rosolphoantimonite, 


8oL  in  HaO  without  decamp,     (Pouget, 
C.  B.  1898,  126.  1793,) 


Cobaltous 
Ppt,    (Pouget,  A,  ch,  1899,  (7)  1*,  554,) 


,  CuSbS<, 


Cuprous 

8oL  in  mixture  of  HNO*  and  tartaric  acid 
with  separation  of  8, 

Insol,  in  NHX)H+Aq,  Decomp,  by  hot 
KOH  and  alkali  sulpUdes+Aq,  (Sommer- 
lad.  /  UlOfC  180^  18.  4.-JO., 

Mm,  Wolfgberite.  SoL  in  HNO,+Aq 
with  separation  of  8  and  Sb*O* 


Cuprous   ^"/o5ulphLajitLm.onite, 

(Somnieriad,  Z,  anorg,  1898, 

Ppt,    InsoL  in  HjO,    Decomp,  by  HjO. 
(Pouget,  A,  ch,  1899,  (7)  18.  556J 

Cuprous  sulphantimonite,  Cu^Bb^r, 
Min.  Guejartie. 

Cupric  <ifM<mipii<iihiiiontte,  Ou  jSb  j3», 
Ppt.    (Pouget,  A,  ch,  1899,  (7)  18.  557.) 


Cuprous 


Min. 
Aq,  and  aqua  regia, 


Decomp,  by  HNO,+ 


Cuprous  potassium  ^tosulphantimonite, 
CujSbS,. 

Ppt,;  easfly  decamp,  by  H^O,    (Pouget, 
r    K.  ]>/^,  129.  JO*.; 

+3HjO,   Fpt.,  deeamp,  by  H^),    (Pou- 
get, A,  ch,  18%,  (7)  18,156,) 


Iron  (ferrous) 


Ppt,     (Pouget,  A,  ch,  1899,  (7)  18,  554,) 
Mui,    HertMehu.     8t  sot  in  Ha+Aq; 
easily  sol.  in  aqua  regia, 


Lead  ^/^fulphflnthnonlte,  Pb,(8bS,)«, 
Ppt,    Very  si.  sol  in  HjO,    Decomp,  by 

Hi),   (Pouget,  A,  ch,  1899,  (7)  18,  553,) 
Min,    tloulfmimte.     Comletely  sot  in 

hot  Ha+Aq;  decamp,  by 


SoL  in  boiling  cone,  HNO*+Aq,  (Pour- 
net.) 

Pb(SbS|U  Min,  Zinekenite.  Decomp. 
by  hot  Hd~f~Aq, 

4PbS,  Sb&,    Min,  PlagionUe. 

2PbS|SbjSf.  Mm,  J&m6it0nU6.  Decamp, 
by  hot  HOl+Aq, 

jrjL^I      «f-    a  %/Kn        \Jl ,ManlvS*tAta 

4JnDD>«  r5Dy5j,      J*im,   JvlfHWyffinUK. 

Min.  Geokronite. 
Min,  Kfori-Jsenite  (7), 


or//«>sulphantimooite, 


Very  sL  soL  in  HjO, 

Decomp.  by  HjO,    (Pouget,  A,  ch,  1899, 
(7)  18.  554,) 

Lead  silver  stilpfaantimoiitte,  ( Afc,  Pb)^b A ,. 
Min, 


Very  *>1. 
71  18.  WD.j 


(Pouget,  A,  ch.  1899, 


Ppt,    (Pouget,  A,  ch,  1899,  (7)  18.  531,) 


Decamp,  by  H^).    (Pouget,  A.  ch,  1899, 
(7)  18.  551.) 


Ppt    SL  soL  in  HA      (Pouget,  A,  ch 
1899,  (7)  18.  553.) 


'-/-'-osuJphantim.onite, 


SL  soL  in  HA    Decomp.  by  HA    (Pou- 
get, A.  ch.  1899,  (7)  18. 553,) 


870 


SULPHANTIMONITE,  NICKEL 


Nickel  or^osulphantimonite,  Ni3Sb2SG. 
Ppt.    (Pouget,  A.  ch.  1899,  (7)  18.  554.) 

Potassium  metosulphantimonite,  KSbS2. 

Insol.  in  cold  H2O.  Decomp.  by  hot  H2O. 
(Pouget,  A.  ch.  1899,  (7)  18.  513.) 

H-l^HaO.  Sol.  in  H2O,  but  decomp. 
quickly. 

Sol.  in  H2O.  (Stanek,  Z.  anorg.  1898,  17. 
119.) 

Potassium  or^osulphantimonite,  K3SbS3. 

Very  deliquescent. 

Very  sol.  in  H2O. 

Decomp.  by  acids.  (Pouget,  A.  ch.  1899, 
(7)  18.  518.) 

Potassium  sulphantimonite,  K2Sb4S7+3H2O. 

SI.  sol.  in  H2O  and  not  decomp.  thereby. 
(Pouget,  A.  ch.  1899,  (7)  18.  522.) 

Decomp.  in  the  air. 

Sol.  in  K2S+Aq.  (Stanek,  Z.  anorg.  1898, 
17.  120.) 

2K2S,  Sb2S3.  Sol.  in  H2O.  (Ditte,  C.  R. 
102.  68.) 

zK2S,  ?/Sb2S3.  Deliquescent.  When  K2S 
is  in  excess,  sol.  in  H2O;  when  Sb2S3  is  in  ex- 
cess, partially  sol.  Aqueous  solution  is  de- 
comp. by  all  acids,  even  CO2,  and  by  K2CO3, 
Na2CQ3,  NaHCO3,  KHCO3,  NH.HCOs+Aq. 
Insol.  in  absolute  alcohol.  (Kohl.) 

Potassium  hydrogen  sulphantimonite, 

KHSb4S7. 
(Pouget,  A.  ch.  1899,  (7)  18.  522.) 

Potassium  silver  or^osulphantimonite, 

Ag2KSbS3. 

Decomp.  by  boiling  H2O.  (Pouget,  C.  R. 
1897,  124.  1519.) 

Potassium  zinc  or^osulphantimonite, 

KZnSbS3. 

Decomp.  by  H2O.  (Pouget,  A.  ch.  1899, 
(7)  18.  552.) 

Silver  or^osulphantimonite,  Ag3SbS3. 

Ppt.  SI.  sol.  in  H2O.  (Pouget,  A.  ch. 
1899,  (7)  18.  547.) 

Min.  Pyrargyrite.  Sol.  in  HNO3+Aq 
with  residue  of  S  and  Sb2O3.  KOH+Aq  dis- 
solves out  Sb2S3. 

Silver  sulphantimomte. 

AgSbS2.    Min.  Miargyrite. 

5Ag2S,  Sb2S3.  Min.  Stephanite.  Easily 
decomp.  by  warm  HNO3-fAq. 

12Ag2S,  Sb2S3.    Min.  Polyargyrite. 

Silver  sodium  or^osulphantimonite, 

Ag2NaSbS3. 

Decomp.  by  H2O.  Pouget,  A.  ch.  1899, 
(7)  18.  551.) 


Sodium  wetosulphantimonite,  NaSbS2. 

Deliquescent.  Decomp.  by  hot  H2O. 
When  Na2S  is  in  excess,  sol.  in  H2O,  but 
partially  sol.  if  Sb2S3  is  in  excess.  (linger, 
Arch.  Pharm.  (2)  148.  1.) 

Ppt.  Insol.  in  H2O.  (Pouget,  C.  R.  1898, 
126.  1145.) 

Sodium  or^Aosulphantimonite,  Na3SbS3 

+9H2O. 

Decomp.  in  solution  in  H2O.  (Pouget, 
C.  R.  1898,  126.  1144.) 

Sodium    sulphantimonite,    Na2Sb4S7+2H2O. 
Sol.  in  H2O.     (Pouget,  C.  R.  1898,  126. 

1145.) 

Na6Sb4S9.    (Pouget,  C.  R.  1898,  126.  1144.) 
4Na2S,    3Sb2S3+3H2O.      Permanent;    sol. 

in  H2O.    Insol.  in  alcohol  and  ether.    (Kohl.) 

Strontium  or^osulphantimonite,  Sr3Sb2Se 

+  10H2O. 

Sol.  in  H2O.  (Pouget,  C.  R.  1898,  126. 
1793.) 

Strontium  py/rosulphantimonite,  Sr2Sb2S6 

+15H2O. 

Sol.  in  H2O  without  essential  decomp. 
(Pouget,  C.  R.  1898,  126.  1793.) 

Zinc  orZAosulphantimonite,  Zn3Sb2S6. 

Ppt.     (Pouget,  A.  ch.  1899,  (7)  18.  552.) 

Ori/iosulpharsenic  acid,  H3AsS4. 

Ppt.    Loses  H2S  by  prolonged  boiling  with 
H2O.    (Nilson,  J.  pr.  (2)  14.  145.) 
See  also  Sulphoxyarsenic  acid: 

Ammonium  sulpharsenate,   (NH4)4As2S7. 

Known  only  in  solution  in  H2O.  Decomp. 
on  boiling  into — 

NH^sSs.    Sol.  in  alcohol. 

(NH4)3AsS4.  Sol.  in  H2O.  Precipitated 
by  alcohol. 

(NH4)2S,  12As2S5.    Ppt.    Insol.  in  H2O. 

Ammonium  magnesium  sulpharsenate, 

(NH4)2S,  MgS,  As2S5. 

Ammonium  sodium  sulpharsenate, 

(NH4)3AsS4,  Na3AsS.. 
Much  more  sol.  in  H2O  than  Na3AsS4;  si. 
sol.  in  cold,  more  sol.  in  hot  alcohol.     (Ber- 
zelius.) 

Barium  sulpharsenate,  Ba(AsS3)2. 

Sol.  in  H2O  and  alcohol.  Decomp.  by 
evaporation. 

Ba2As2S7.  Sol.  in  H2O  in  all  proportions 
with  decomp.  Decomp.  by  alcohol. 

Ba3(AsS4)2.  Sol.  in  H2O.  Insol.  in  alco- 
hol. 

BaS,  3As2S5.     Ppt.     Insol.  in  H2O. 


SULPHARSENATE,  SODIUM  ZINC 


871 


Barium  potassium  sulpharsenate, 
KBaAsS4+6H2O. 

Easily  sol.  in  H2O. 

Decomp.  by  acids  with  separation  of  As2S5. 
(Glatzel,  Z.  anorg.  1911,  71.  209.) 

Barium  sulpharsenate  sulpharsenite, 

Ba3(AsS4)2,  Ba2As2S5-f4H2O. 
SI.  sol.  in  cold,  more  easily  in  hot  H2O. 
(Nilson.) 

Bismuth  sulpharsenate,  2Bi2S3,  3As2S6. 
Sol.  in  Na3AsS4+Aq. 
Bi2S3,    3As2S5.      As    above.      (Berzelius.) 

Cadmium  sulpharsenate. 
Ppt.     (Berzelius,  Pogg.  7.  88.) 

Calcium  sulpharsenate,  Ca2As2S7. 

Sol.  in  H2O  and  alcohol. 

Ca3(AsS4)2.  Easily  sol.  in  H2O.  Insol.  in 
alcohol. 

+10H2O.  Easily  sol.  in  H2O.  (Nilson,  J. 
pr.  (2)  14.  169.) 

5CaS,  2AsS2S6+6H2O.  Easily  sol.  in  H2O. 
(Nilson,,  J.  pr.  (2)  14.  163.) 

Cerous  sulpharsenate,  Ce2As2S7. 
Ppt. 

Ce3(AsS4)2.    Ppt. 
Ce4(As2S7)3.     Ppt. 

Cobaltous  sulpharsenate,  Co2As2S7. 

Ppt.  Sol.  in  excess  of  sodium  sulpharsen- 
ate +Aq. 

Cuprous  sulpharsenate,  Cu3AsS4. 

Ppt.     (Preis,  A.  267.  201.) 

Min.  Enargite.  Clarite.  Not  wholly  de- 
comp.  by  HCl+Aq.  Sol.  in  HCl+Aq  with 
residue  of  As2O3.  Not  attacked  by  KOH + Aq. 

Cupric  sulpharsenate,  Cu2As2S7. 

Ppt.  Sol.  in  (NH4)2S+Aq.  Decomp.  by 
NH4OH+Aq.  (BerzeUus.) 

Cu3(AsS4)2.     Ppt.      (Preis,   A.  267.   201.) 

Glucinum  sulpharsenate. 
SI.  sol.  in  H2O. 

Gold  sulpharsenate,  AuAsS4. 
Sol.  in  pure  H2O.    Insol.  in  NasAsS4+Aq. 
2Au2S3,  3As2S5.    Sol.  in  H2O.    (Berzelius.) 

Iron  (ferrous)  sulpharsenate,  Fe2As2S7. 

Ppt.     Sol.  in  Na;jAsS4+Aq.     (Berzelius.) 

Iron    (ferric)    sulpharsenate,    Fe4(As2S7)3. 
Ppt.     Sol.  in  NasAsS4+Aq.     (Berzelius.) 

Lead  sulpharsenate,  Pb2As2S7. 
Ppt.    (Berzelius.) 
Pb3(AsS4)2.    Ppt. 


Lithium  sulpharsenate,  Li3AsS4. 

Easily  sol.  in  hot,  less  sol.  in  cold  H2O. 
Insol.  in  alcohol. 

Li4As2S7.  Comoletely  sol.  in  H2O.  De- 
comp. by  alcohol. 

LiAsS3.    Known  only  in  acid  solution. 

Magnesium  sulpharsenate,  Mg2As2S7. 

Sol.  in  all  proportions  of  H2O,  and  in  al- 
cohol. 

Mg3(AsS4)2.  Sol.  in  H2O.  Decomp. 
alcohol. 

3MgS,  As2S5.    Nearly  insol.  in  H2O. 

5MgS,  2As2S5-M5H2O.  Very  sol.  in  H20. 
(Nilson.) 

Manganous  sulpharsenate,  Mn2As2S7. 
SI.  sol.  in  H2O. 

Mn3(AsS4)2.    Permanent.    SI.  sol.  in  H2O. 
6MnS,  As2S5.    SI.  sol.  in  H2O. 

Mercurous  sulpharsenate,  (Hg2)2As2S7. 
Ppt. 

Mercuric  sulpharsenate,  Hg2As2S7. 
Ppt.     (Berzelius,  Pogg.  7.  29.) 
Hg3(AsS4)2.     Ppt.     (Preis,  A.  257.   200.) 

Nickel  sulpharsenate,  Ni3(AsS4)2. 
Ppt.    Not  decomp.  by  HCl+Aq.    Sol.  in 

Na3AsS4+Aq.     (Berzelius.) 
2MS,  As2£*6.    As  above. 

Potassium  sulpharsenate,  KAsS3. 

Known  only  in  alcoholic  solution. 

K4As2S7.  Deliquescent.  Sol.  in  H20,  from 
which  alcohol  ppts.  K3AsS4. 

K3AsS4.  .Deliquescent.  Very  sol.  in  H2O, 
from  which  it  is  precipitated  by  alcohol. 

+H2O.  Very  deliquescent.  (ISilson,  J. 
pr.  (2)  14.  159.) 

Potassium  sodium  sulpharsenate. 
Sol.  hi  H2O. 

Silver  sulpharsenate,  AgsAsS4. 
Ppt.     (Berzelius,  Pogg.  7.  29.) 
Ag2As2S7.     Ppt. 

Sodium  sulpharsenate,  NaAsS3. 

Known  only  in  alcoholic  solution. 

Na^sszS?.  Sol.  in  H20.  Alcohol  ppts. 
Na3AsS4  from  H2O  solution. 

Na3AsS4+7^H2O.  Easily  sol.  in  H2Q, 
from  which  it  is  precipitated  by  alcohol. 

+8H2O.  Insol.  in  alcohol;  very  sol.  in 
H2O.  (McCay,  Z.  anal.  1895,  34.  726.) 

+9H2O.    (Nilson,  J.  pr.  (2)  14.  160.) 

Na2S,  12As2S5  (?).    Insol.  in  H2O. 

Sodium    zinc    sulpharsenate,    NaZnAsS4  + 

4H20. 

Sol.  in  hot  H2O  with  decomp.  (Preis,  A. 
257.  202.) 


872 


SULPHARSENATE,  STRONTIUM 


Strontium   sulpharsenate,   Sr3(AsS4)2. 

Easily  sol.  in  H2O;  insol.  in  alcohol. 

Sr2As2S7.  Easily  sol.  in  H2O,  from  which 
alcohol  ppts.  Sr3(AsS4)2. 

Strontium  sulpharsenate  sulpharsenite, 

Sr3(AsS4)2,   Sr2As2S5+4H2O. 
Easily  sol.  in  H2O.    (Nilson,  J.  pr.  (2)  14. 
162.) 

Thallous  sulpharsenate,  Tl3AsS4. 

Not  decomp.  by  H2O.  Decomp.  by  dil. 
acids.  Insol.  in  dil.  alkali  sulphides.  Par- 
tially decomp.  by  boiling  with  a  cone,  solu- 
tion of  sodium  sulphide.  (Hawley,  J.  Am. 
Chem.  Soc.  1907,  29.  1013.) 

Tin  (stannous)  sulpharsenate.. 
Ppt. 

Tin  (stannic)  sulpharsenate. 
Ppt. 

Uranic  sulpharsenate,  2U2S3,  As2S5. 
Ppt.    Sol.  in  Na3AsS4+Aq. 

Zinc  sulpharsenate,  Zn3(AsS4)2. 
Ppt.     (Berzelius.) 
2ZnS,  As2S5.    Ppt.    (Berzelius.) 
ZnS,  As2S5.    (Wohler.) 

ZH'sulpharsenic  acid. 

See  ZKsulphoxyarsenic  acid. 

Sulpharseniosulphomolybdic  acid. 

Ammonium  sulpharseniosulphomolybdate, 

(NH4)4As2S7(MoS3)2+5H2O. ' 
Very  unstable. 

Sol.  in  H2O  with  decomp.  (Weinland,  Z. 
anorg.  1897,  16.  49.) 

Barium ,  Ba2As2S7(MoS3)2+14H2O. 

Sol.  in  H2O  with  decomp.     (Weinland.) 

Potassium ,  KAsS3(MoS3) +4H2O. 

(Weinland.) 

K4As2S7(MoS3)2+8H2O.  Sol.  in  H2O. 
Decomp.  by  mineral  acids.  Insol.  in  alcohol. 
(Weinland.) 

Sodium ,  NaAsS3(MoS3)+6H2O. 

Insol.  in  H2O.  Easily  sol.  in  dil.  NaOH 
andNH3+Aq.  (Weinland.) 

Na4As2S7(MoS3)2+14H2O.  Sol.  in  H2O. 
Decomp.  by  mineral  acids.  (Weinland.) 

Sulpharseniosulphoxymolybdic  acid. 

Barium  sulpharseniosulphoxymolybdate,  . 

Ba2As2S7(Mo2S3O3)  +  12H2O. 
Sol.  in  H2O.     (Weinland,  Z.  anorg.  1897, 
16.  60.) 


Magnesium  sulpharseniosulphoxymolybdate, 

Mg2As2S7(Mo2S3O3)  +16H2O. 
Very  sol.  in  H2O.    (Weinland.) 

Potassium ,  KAsS3(MoSO2)+2^H2O. 

Sol.  in  H2O  with  decomp.    (Weinland.) 
K4As2S7(Mo2S3O3)+6H2O.     Very   sol.   in 

H2O.    Weinland.) 

+10H2O.     (Weinland.) 

Sodium ,  NaAsS3(MoSO2)+5H2O. 

SI.  sol.  in  cold,  very  sol.  in  hot  H2O.  (Wein- 
land.) 

Na4As2S7(Mo2S3O3)+15H2O.  Very  sol. 
inH2O.  (Weinland.) 

Sulpharsenious  acid. 

Ammonium  sulpharsenite,  NH4As3S5+2H2O. 

Insol.  in  H2O.  Ppt.  Sol.  in  KOH  or 
NH4OH+Aq.  SI.  attacked  by  boiling  HC1+ 
Aq.  (Nilson,  J.  pr.  (2)  14.  42.) 

(NH4)4As2S5  =  2(NH4)2S,  As2S3.  Sol.  in 
H2O,  from  which  alcohol  ppts.  (NH4)3AsS3. 

(NH4)3AsS3  =  3(NH4)2S,  As2S3.  Decomp. 
on  air;  sol.  in  H2O.  Insol.  in  alcohol. 

(NH4)5As3S10.  Sol.  in  H2O.  (Nilson,  J. 
pr.  (2)  14.  160.) 


Barium  sulpharsenite,  Ba2As2S5. 
SI.  sol.  in  H2O.  Decomp.  by  ; 
+5H2O.  SI.  sol.  in  H2O.  (Nilson,  J.  pr. 


SI.  sol.  in  H2O.    Decomp.  by  alcohol. 

H20. 
(2)  14.  46.) 


+15H2O.    SI.  sol.  in  cold  H2O.     (Nilson.) 

Ba3(AsS3)2.  SI.  sol.  in  H2O.  Precipitated 
by  alcohol. 

+  14H2O.  SI.  sol.  in  cold,  easily  in  hot 
H2O.  (Nilson.) 

Ba(AsS2)2+2H2O.  Insol.  in  H2O.  (Nil- 
son,  J.  pr.  (2)  14.  44.) 

BaAsi2Si9.     Insol.  in  HCl+Aq.     (Nilson.) 

Bismuth  sulpharsenite,  2Bi2S3,  As2S3. 
Ppt. 

Cadmium  sulpharsenite. 

Ppt.    (Berzelius,  Pogg.  7.  146.) 

Calcium  sulpharsenite,  Ca2As2S5. 

Sol.  in  H2O,  from  which  alcohol  ppts. 
Ca3(AsS3)2. 

Ca3(AsS3)2.    Sol.  inH2O. 

+  15H2O.    Precipitated  by  alcohol. 

Ca(AsS2)2+10H2O.  Sol.  in  H2O.  (Nilson, 
J.  pr.  (2)  14.  54.) 

CaAs8S13+10H2O  (?).  Insol.  in  cold  H2O. 
Decomp.  by  hot  H2O.  (Nilson.) 

CaAsi8S28  +  10H2O  (?).  SI.  sol.  in  hot  H2O. 
(Nilson.) 

Ca7As2S10+25H2O.  SI.  sol.  in  cold  or  hot 
H2O.  (Nilson.) 

Cerous  sulpharsenite,  Ce2As2S6. 
Ppt. 


SULPHARSENITE,  URANIC 


873 


Chromic  sulpharsenite,  2Cr2S3,  3As2S3. 
Ppt.    Insol.  in  Na2S+Aq. 

Cobaltous  sulpharsenite,  2CoS,  As2S3. 

Ppt.  Sol.  in  excess  of  sodium  sulpharsen- 
ite+Aq. 

Cuprous  sulpharsenite, 

3Cu2S,  2As2S3  =  Cu5As4S9. 

Min.  Binnile.  Decomp.  by  hot  acids  and 
KOH+Aq. 

2Cu2S,  As2S3  =  Cu4As2S5.  Decomp.  by 
acids,  KOH  and  K2S+Aq.  (Sommerlad,  Z. 
anorg.  1898,  18.  434.) 

Cupric  sulpharsenite,  Cu3AsS3. 

Insol.  in  H20  or  HCl+Aq.  Sol.  in  Na3AsS3 
+Aq. 

Cu2As2S5.    Ppt.    (Berzelius.) 

Glucinum  sulpharsenite,  2G1S,  As2S8. 

Ppt.  Sol.  in  acids;  partly  sol.  in  NH4OH 
+Aq. 

Gold  sulpharsenite,  2Au2S3,  3As2S3. 
Ppt.    (Berzelius.) 

Iron  (ferrous)  sulpharsenite. 
Ppt.    Sol.  in  Na3AsS3+Aq.    (Berzelius.) 

Iron  (ferric)  sulpharsenite. 

Ppt.  Sol.  in  excess  of  a  ferric  salt,  or 
Na3AsS3+Aq.  (Berzelius.) 

Lead  sulpharsenite,  Pb2As2S5. 
Ppt.    Min.  Dufreynosite. 
Pb(AsS2)2  =  PbS,  As2S3.     Min.     Sartorite. 
Pb4As2S7.    Min.  Jordanite. 

Lithium  sulpharsenites. 
Resemble  K  salts. 

Magnesium  sulpharsenite,  Mg2As2S6. 

Almost  completely  sol.  in  H2O.  Easily  sol. 
in  alcohol.  (Berzelius.) 

+8H2O.    SI.  sol.  in  H2O.    (Nilson.) 

Mg(AsS2)2+5H2O.  Slowly  sol.  in  both 
cold  and  hot  H2O.  (Nilson,  J.  pr.  (2)  14. 
59.) 

Mg3(AsS3)2+9H2O.     (Nilson.) 

Manganous  sulpharsenite,  Mn2As2S6. 
Ppt.    Decomp.  by  HCl+Aq. 

Mercurous  sulpharsenite,  (Hg2)2As2S5. 
Ppt.    (Berzelius.) 

Mercuric  sulpharsenite,  Hg2As2S5. 
Ppt. 
Hg(AsS2)2.    Ppt.    (Berzelius,  Pogg.  7.  149.) 

Nickel  sulpharsenite,  Ni3(AsS3)2. 
Ppt.    (Berzelius.) 


Platinum  sulpharsenite,  Pt2As2S5. 
Ppt. 

Potassium  sulpharsenite,  K4As2S5. 

Decomp.  by  H2O  or  alcohol.     (Berzelius.) 

K3AsS3.  Sol.  in  H2O.  Insol.  in  alcohol. 
(Berzelius.) 

K2As4S7.  Sol.  in  H2O  and  alcohol.  (Ber- 
zelius.) 

K2AsS2.    Decomp.  by  H2O.    (Berzelius.) 

+2^H2O.  Not  wholly  sol.  in  H2O.  (Nil- 
son,  J.  pr.  (2)  14.  30.) 

K-As4S3  +8H2O.     (Nilson.) 

KAs3S5+H2O.  Insol.  in  H2O.  Slowly  at- 
tacked by  hot  HCl+Aq.  Sol.  in  KOH+Aq. 
(Nilson.) 

Silver  sulpharsenite,  12Ag2S,  As2S3. 

Ppt.  (Sommerlad,  Z.  anorg.  1898,  18. 
428.) 

5Ag2S,  As2S3=Ag5AsS4.    (Sommerlad.) 

Ag3AsS3.  Min.  Proustite.  'Sol.  in  HNO3  + 
Aq.  KOH+Aq  dissolves  out  Sb2S3.  (Senar- 
mont,  A.  ch.  (3)  32.  129;  Wohler,  A.  27.  159.) 

2Ag2S,  As2S3.  Partially  sol.  in  HNO3+ 
Aq.  (Berzelius.) 

AgAsS2.    (Berzelius,  Pogg.  7.  150.) 


Sodium  sulpharsenite, 

Attacked  by  HCl+Aq  with  difficulty. 
(Nilson,  J.  pr.  (2)  14.  37.) 

+  1  ^H2O.  Forms  coagulum  with  cold,  sol. 
in  hot  H2O.  (Nilson.) 

Na2As4S7+6H2O.  Sol.  in  much  H2O;  not 
easily  decomp.  by  HCl+Aq.  (Nilson.) 

NaAs3S5+4H2O.  Ppt.  (Nilson,  J.  pr.  (2) 
14.  3.) 

Strontium    sulpharsenite,    3SrS,    As2S3  + 
15H2O. 

Sol.  in  H2O+Aq;  insol.  in  alcohol.  (Voigt 
and  Gottling.) 

2SrS,  As2S3.  Sol.  in  H2O;  decomp.  by 
alcohol. 

+15H2O.    (Nilson,  J.  pr.  (2)  14.  53.) 

Sr(AsS2)2+23/6H2O.  SI.  sol.  in  H2O.  (Nil- 
son.) 

Thallous  sulpharsenite,  TlAsS2. 

Ppt.  Decomp.  by  KOH+Aq.  (Gunning, 
J.  B.  1868.  247.) 

Above  compound  is  a  mixture  of  As2S3  and 
T12S.  (Hawley,  J.  Am.  Chem.  Soc.  1907, 
29.  1012.) 

Min.  Lorandite.  (Kuenner  and  Loezka, 
C.  C.  1904,  II.  844.) 

Tin  (stannous)  sulpharsenite,  Sn2As2S5. 
Ppt. 

Tin  (stannic)  sulpharsenite,  SnAs2S6. 
Ppt.    (Berzelius,  Pogg.  7.  147.) 

Uranic  sulpharsenite,  2U2S3,  As2S3. 
Ppt. 


874 


SULPHARSENITE,  ZINC 


Zinc  sulpharsenite. 

Ppt.    (Berzelius,  Pogg.  7.  145.) 

Zirconium  sulpharsenite,  2Zr2S3,  As2S3. 

Ppt.  Insol.  in  solutions  of  alkali  sulph- 
arsenites.  SI.  sol.  in  Na2S  Aq.  Not  de- 
comp.  by  acids.  (Berzelius.) 

"  Sulphatammon,"  2NH3,  SO3. 

(Rose.) 

Is  ammonium  imidosulphonate,  which  see. 
(Berglund.) 

"Parasulphatammon,"  3NH3,  2SO3. 

(Rose.) 

Is  basic  ammonium  imidosulphonate,  which 
see.  (Berglund.) 

Sulphatoiodic  acid. 

Potassium  sulphatoiodate,  K2H03SIO4  or 
KIO,,  KHS04. 

Decomp.  by  H2O.  (Blomstrand,  J.  pr.  (2) 
40.  317.) 

See  lodate  sulphate,  potassium. 

Sulphatooctamine  cobaltic  carbonate 

(SO4)2Co2(NH3)8CO3+4H2O. 

Sol.  in  H2C.  (Vortmann  and  Blasberg,  B. 
22.  2650.) 

(SO4)Co2(NH3)8(C03)2+3H2O.  Sol.  in 
H2O.  (V.  andB.) 

See  Carbonatotetramine  cobaltic  sulphate. 
(Jorgensen.) 


Sulphatoplatinamine  sulphate, 

S04Pt(NH3)2S04+3H20. 
Easily  sol.  in  H20.     Sol.  in 


Sulphatoplatincfo'amine  sulphate, 

SO4Pt(N2H6)2SO4+H2O. 
Insol.  in  H2O. 

Sulphatopurpureocobaltic  bromide, 

Co(SO4)(NH3)5Br. 

Sol.  in  H2O,  from  which  it  is  precipitated 
by  cone.  HBr+Aq.  (Jorgensen,  J.  pr.  (2) 
26.  94.) 

-  carbonate,  [(SO4)Co(NH3)6]2CO3  + 
4H20. 

Sol.  in  H2O.  (Vortmann  and  Blasberg,  B. 
22.  2648.) 

-  chloroplatinate,  2Co(SO4)(NH3)6Cl, 
PtCl4+2H2O. 

SI.  sol.  in  cold  H2O.    (Jorgensen.) 

-  nitrate,  Co(SO4)(NH3)6(NO8). 
Somewhat  si.  sol.  in  cold  H2O.    (Jorgensen.) 


Sulphatopurpureocobaltic  sulphate. 

[Co(S04)(NH3)5]2S04+H20. 

Very  easily  sol.  in  H2O.  (Jorgensen,  J.  pr. 
(2)  26.  94.) 

Co(S04)NH3)5(HS04)+2H20.  Sol.  in 
about  25  pts.  of  cold  H2O.  Sol.  in  dil.,  insol. 
in  cone.  NH4OH-f-Aq.  (Jorgensen.) 

Sulphazic  acid,  H4S2N2O9  = 

SO3H— N(OH)—  O— N—  (OH)SO3H. 
Known  only  in  its  salts.    (Raschig,  A.  241. 
161.) 

Potassium  sulphazate,  K3HS2N2O9  = 

(S03K)(OK)N-^0— N(OH)— (S03K). 
Sol.   in  H2O,   but  decomp.   on  standing. 
(Raschig,  A.  241.  161.) 

Sulphazidic  acid. 
(Fremy.) 
See  Hydroxylamine  monosulphonic  acid. 

Sulphazilinic  acid. 
See  Oxysulphazotic  acid. 

Afetasulphazilinic  acid. 
See  Tnsulphoxyazotic  acid. 

Sulphazinous  acid. 

(Fremy.) 

See  Dihydroxylamine  sulphonic  acid. 

Sulphazotic  acid,  H6N2S4Oi4  = 

(SO3H)3=NH— NO  =  OH(SO3H). 
Known  only  in  its  salts.     (Glaus,  A.  158. 
52  and  194).    Has  the  formula 

(S03H)2NH<g>NH(S03H)2. 
(Raschig,  A.  241.  161.) 

Lead  potassium  sulphazotate. 

Insol.  in  cold,  decomp.  by  hot  H2O.  Insol. 
in  alcohol  and  ether.  (Fremy,  A.  ch.  (3)  16. 
439.) 

Potassium  sulphazotate,  K5HN2S4Oi4-}-H2O 
=  (SO3K)2NK  <£>  NH(SO3K)2. 

Very  sol.  in  hot,  less  in  cold  H2O.     (Ras- 

ig,  A.  241.  161.)  Decomp.  gradually  by 
boiling.  (Glaus.)  Insol.  in  alcohol  or  ether. 
(Fremy,  A.  ch.  (3)  16.  428.) 

True  composition  is  HON(SO3K)2, 
KON(SO3K)2+H2O.  Potassium  hydroxyl- 
amine  disulphonate.  (Divers  and  Haga, 
Chem.  Soc.  1900,  77.  432.) 

Forms  basic  salt 

(SO3K)2NK<^>NK(SO3K)2,        which      is 
easily  sol.  and  decomp.  by  H2O.     (Raschig.) 

Potassium    sodium    sulphazotate, 

K4NaHN2S4O14+2H2O. 
Quite  easily  sol.   in   H2O.      (Raschig,   A. 
241.  161.) 


SULPHOCHROMIC  ACID 


875 


Disulphhydroxy azotic  acid,  ONH(SO2H)3. 
Known  only  in  its  salts.  (Glaus,  A.  158. 
52  and  194.)  Correct  composition  is  hydroxy- 
lamine  sulphonic  acid  HON(SO3H)2,  which 
see.  (Raschig,  A.  241.  161.) 

Sulphhydroxylamic  acid. 

(Glaus.) 

See  Hydroxylamine  wonosulphonic  acid. 

Disulphhydroxyazotic  acid. 
(Glaus.) 
See  Hydroxylamine  disulphonic  acid. 

Sulphides. 

The  sulphides  of  the  alkali  metals  are  spl.  in 
H2O;  those  of  the  alkali-earth  metals  are 
much  less  sol.,  and  are  decomp.  upon  solution 
into  hydrosulphide  and  hydroxide. 

The  other  sulphides  are  insol.  in  H2O. 

For  each  sulphide,  see  under  the  respective 
element. 

Sulphimide,.SO2NH. 
See  Imidosulphamide. 


TYisulphimide, 

(SO2NH)3. 

Sol.  in  methyl  alcohol;  si.  sol.  in  ether; 
insol.  in  chloroform  and  benzene.  (Hantzsch 
B.  1901,  34.  3440.) 

Ammonium  sulphimide,  SO2N(NH4). 
Sol.  in  H2O;  insol.  in  alcohol.    (Traube.) 

Barium ,  (SO2N)2Ba+2H2O. 

Sol.  in  H2O.    (Traube.) 

Potassium ,  SO2NK. 

Not  very  sol.  in  H2O. 

Silver  — ,  SO2NAg. 

Sol.  in  500-600  pts.  cold,  more  easily  in 
hot  H2O.  Sol.  in  acids. 

Sodium ,  SO2NNa. 

Ver}'  sol.  in  H2O. 

"  Sulphitammon,"  NH3,  SO2. 
See  Thionamic  acid. 

Sulphobismuthous  acid. 

Cuprous  sulphobismuthite,  AuBiS2. 

Min.  Emplectite.    Sol.  in  HNO3+Aq. 

Cu6Bi4S9.  Min.  Klaprothite.  Completely 
sol.inHCl+Aq. 

Cu3BiS3.  Min.  Wittichenite.  Sol.  in  HC1 
-f  Aq  and  in  HNO3+Aq. 


Cuprous  lead  sulphobismuthite,  Cu2S,  2PbS, 
Bi2S3. 

Min.  Patrinite. 

Sol.  in  HNOs+Aq  with  residue  of  S  and 
PbSO4. 

Lead ,  2PbS,  Bi2S3. 

Min.   Cosalite. 

2PbS,  3Bi2S3.    Min.  Chiviatite. 

Potassium ,  KBiS. 

Decomp.  by  H2O. 

Sol.  in  HCl+Aq.  (Schneider,  Pogg.  1869, 
136.  464.) 

Metasulphoboric  acid,  B2S3H2S. 

Decomp.  by  H2O  and  alcohol. 

1  pt.  is  sol.  in  5  pts.  benzene 

1  pt.  is     "   "  5     "    CS2 

Very  si.  sol.  in  CS2  at -20°.  (Stock,  B. 
1901,  34.  401.) 

Sulphocarbonic  acid. 

Ammonium    cuprous    sulphocarbonate, 

CS3CuNH4. 

This  salt  was  formerly  described  as  cupric 
sulphocarbonate  ammonia,  CS3Cu,  NH3. 
(Hofmann,  B.  1903,  36.  1146.) 

Cuprous    potassium    sulphocarbonate, 
CS3CuK. 

Nearly  insol.  in  cold  H2O. 

Somewhat  sol.  in  hot  H2O,  NaOH  and 
NH4OH+Aq.  (Hofmann.) 

Cupric    sulphocarbonate    ammonia,    CS3Cu, 

NH3. 

Very  si.  sol.  in  strong  NH4OH+Aq.;  insol. 
in  cold  H2O,  si.  sol.  in  hot  H2O.  (Hofmann, 
Z.  anorg.  1897,  14.  295.) 

Is  ammonium  cuprous  sulphocarbonate. 
(Hofmann,  B.  1903,  36.  1146.) 

• 
Cuprous  sulphocarbonate  potassium  cyanide, 

CS3Cu2,  2KCN+2H2O. 
Sol.  in  H2O  and  dil.  alkalies  on  warming. 
(Hofmann,  B.  1903,  36.  1148.) 

Zinc  sulphocarbonate  ammonia, 

CS3Zn,  2NH3. 
Ppt.    (Hofmann,  Z.  anorg.  1897, 14.  277.) 

Sulphochromic  acid,  H2CrO4,  SO3.  (?). 
Sol.  in  H2O.     (Bolley,  A.  66.  113.) 
(SO3)4Cr2O2(OH)2.    Sol.  in  H2O.    All  salts 

iven  alkali  salts  are  insol.  in  H2O.    (Recoura, 

Bull.  Soc.  1896,  (3)  15.  315.) 

[Cr2O2(OH)4(SO2)4O3,        Cr2O(OH)2(SO2)3 

(OH)>](OH)2.      Sol.    in    H2O.      (Wyrouboff, 

Bull.  Soc.  1902,  (3)  27.  721.) 


876 


SULPHOCHROMATE,  CHROMIUM 


Chromium   sulphochromate, 

Cr2O2(OH)4(SO2)4O2(OH)2Cr2(OH)6. 
Ppt.;  decomp.  by  boiling  H2O.     (Wyrou- 
boff,  Bull.  Soc.  1902,  (3)  27.  720.) 

Sulphochromous  acid. 

Ferrous  sulphochromite,  FeCr2S4. 

Insol.  in  H2O,  and  nearly  so  in  HCl+Aq. 
(Groger,  W.  A.  B.  81,  2.  531.) 

Manganous  — — •,  MnCr2S4. 
Insol.  in  H2O  and  HCl+Aq.     (Groger.) 

Potassium -,  K2Cr2S4. 

Insol.  in  H2O  and  in  hot  HCl+Aq. 

Easily  sol.  in  aqua  regia  .  Slowly  sol.  in 
cold,  rapidly  sol.  in  hot  dil.  HNO3+Aq. 
(Milbauer,  Z.  anorg.  1904,  42.  443.) 

K2Cr4S7.  Stable  in  the  air;  sol.  in  HNO3 
and  aqua  regia  with  decomp.  (Schneider, 
J.  pr.  1897,  (3)  66.  407.) 

Silver ,  Ag2Cr2S4. 

Not  attacked  by  HCl+Aq  even  on  heat- 
ing. Decomp.  by  cone.  HN03.  (Schneider, 
J.  pr.  1897,  (2)  66.  401.) 

Sodium ,  Na2Cr2S4. 

Insol.  in  H2O.  SI.  attacked  by  dil.  HC1  or 
H2SO4+Aq.  Sol.  in  cold  cone.  HNO3  or 
aqua  regia.  Sol.  in  hot  dil.  HNO3+Aq. 
(Groger.) 

Sol.  in  acids  with  decomp.  (Schneider, 
J.  pr.  1897,  (3)  56.  415.) 

Zinc ,  ZnCr2S4. 

Insol.  in  H2O:  sol.  in  traces  in  boiling  cone. 
HC1  or  dil.  H2SO4+Aq;  sol.  in  HNO3+Aq 
(Groger,  W.  A.  B.  81,  2.  531.) 

Sulphocyanhydric  acid,  HSCN. 

Sol.  in  H2O. 

Sat.  HSCN+Aq  hag  sp.  gr.  =  1.022.  (Por- 
rett,  1814.)  HSCN+Aq  containing  12.7% 
HSCN  has  sp.  gr.  1.040  at  12.7°.  (Hermes 
Z.  Ch.  1866.  417.) 

Sulphocyanides. 

Most  sulphocyanides  are  sol.  in  H2O,  bu1 
Cu,  Pb,  Hg,  and  Ag  sulphocyanides  are  insol 

Aluminum  sulphocyanide,  A1(SCN)3. 

Known  only  in  solution. 

A1(SCN)2(OH)4.  Known  only  in  solution 
(Suida.) 

Aluminum  potassium  sulphocyanide, 

K3Al(SCN)e+4H2O. 
Very  hydroscopic. 

Sol.  in  H2O  and  alcohol.  (Rosenheim,  Z 
anorg.  1901,  27.  302.) 


Ammonium  sulphocyanide,  NH4SCN. 

Deliquescent,  and  very  sol.  in  H2O. 

100  pts.  H2O  dissolve  128.1  pts.  at  0°  and 
162.2  pts.  at  20°. 

NH4SCN+Aq  sat.  at  ord.  temp,  has 
density  of  1.138  and  100  cc.  contains  69.16  g. 
NH4SCN.  (Klason,  J.  pr.  1887,  (2)  36.  67.) 

By  dissolving  90  g.  NH4SCN  in  90  g.  H2O 
at  17°,  the  temp,  falls  to  —12°.  (Clowes,  Z. 
3h.  1866.  190.) 

133  pts.  NH4SCN+100  pts.  H2O  at  13.2° 
.ower  the  temp.  31.2°.  (Riidorff,  B.  2.  68.) 

Sol.  in  liquid  SO2.  (Walden,  B.  1899,  32. 
2864.) 

Difficultly  sol.  in  AsBr3.  (Walden,  Z. 
anorg.  1902,  29.  374.) 

Very  easily  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  826.) 

Easily  sol.  in  alcohol. 

Easily  sol.  in  acetone.    (Krug  and  M'Elrpy. 

SI.  sol.  in  benzonitrile.  (Naumann,  B: 
1914,  47.  1369.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3789.) 

Difficultly  sol.  in  ethyl  acetate.  (Nau- 
mann, B.  1910,  43.  314.) 

Ammonium  bismuth  sulphocyanide, 

(NH4)3Bi(SCN)3. 

As*K  salt.  (Rosenheim  and  Vogelgesang 
Z.  anorg.  1906,  48.  215.) 

Ammonium  cadmium  sulphocyanide, 

(NH4)2Cd(SCN)4+2H2O. 
Somewhat  deliquescent.         , 
Melts  in  crystal  H2O  at  25°. 
Insol.  in  alcohol.     (Grossmann,  B.   1902, 
35.  2667.) 

Ammonium   cadmium    molybdenyl    sulpho- 
cyanide,         NH4SCN,          Cd(SCN)2, 
Mo(OH)(SCN)3+3H2O. 
(Maas  and  Sand,  B.  1908,  41.  1513.) 

Ammonium  cobaltous  sulphocyanide, 

(NH4)2Co(SCN)4. 

Decomp.  in  moist  air. 

Cannot  be  recryst.  from  H2O.  (Treadwell, 
Z.  anorg.  1901,  26.  109.) 

+4H2O.    Sol.  in  H2O. 

Sol.  in  methyl,  ethyl  and  amyl  alcohol, 
in  acetone  and  in  ether  +  Aq. 

Can  be  recryst.  from  H2O  or  alcohol  with- 
out decomp.  (Rosenheim  and  Cohn,  Z. 
anorg.  1901,  27.  289.) 

Ammonium  iron  (ferric)  sulphocyanide, 
9NH4SCN,  Fe(SCN)3+4H2O. 

Deliquescent,  and  sol.  in  H2O.  (Kriiss  and 
Moraht,  A.  260.  207.) 

3NH4SCN,  Fe(SCN)3.  Extremely  deli- 
quescent. 

Ammonium  mercuric  sulphocyanide, 

2NH4SCN,  Hg(SCN)2. 
Easily  sol.  in  H2O.     (Fleischer,   A.   179. 
228.) 


SULPHOCYANIDE,  BISMUTH 


877 


NH4Hg(SCN)3.  Insol.  in  cold;  sol.  in  hot 
H2O.  (Rosenheim,  Z.  anorg.  1901,  27. 284.) 

Ammonium  molybdenyl  sulphocyanide, 

3NH4SCN,    Mo(OH)(SCN)3+3H2O. 
(Sand  and  Maas,  B.  1907,  40.  4507.) 

Ammonium  nickel  sulphocyanide, 

(NH4)4Ni(SCN)6+4H2O. 
Sol.  in  H2O  with  decomp. 
SI.  sol.  in  cold;  easily  sol.  in  hot  alcohol. 
(Rosenheim,  Z.  anorg.  1901,  27.  292.) 

Ammonium  silver  sulphocyanide,  NH4SCN, 

AgSCN. 
Decomp.  by  H2O. 

Ammonium  vanadium  sulphocyanide, 

V(SCN)3,  3NH4SCN+4H2O. 
Sol.  in  H2O;  sol.  in  alcohol;  si.  sol.  in  ether. 
(Ciocci,  Z.  anorg.  1898, 19.  311.) 

Ammonium  vanadyl  sulphocyanide, 

(NH4)2VO(SCN)4+5H2O. 

Sol.  in  H2O,  alcohol,  ether,  acetone,  amyl 
alcohol  and  ethyl  acetate.  (Koppel,  Z. 
anorg.  1903,  36.  290.) 

Ammonium  zinc  sulphocyanide, 

(NH4)  2Zn(SCN)  4 +3H2O. 

Easily  sol.  in  H2O  and  in  alcohol.  (Walden, 
Z.  anorg.  1900,  23.  374.) 

+4H2O.  Easily  sol.  in  cold  H2O,  acetone, 
alcohols  and  ether.  (Rosenheim  and  Huld- 
schinsky,  B.  1901,  34.  3913.) 

Ammonium  sulphocyanide  mercuric  bromide, 
NH4SCN,  HgBr2. 

Very  sol.  in  H2O. 

Sol.  in  alcohol.  (Grossmann,  B.  1902,  35. 
2945.) 

2NH4SCN,  HgBr2+H2O.  Somewhat  de- 
liquescent. 

Very  sol.  in  H2O. 

Sol.  in  alcohol.     (Grossmann.) 

Arsenic  sulphocyanide,  As(SCN)3. 

Decomp.  by  H2O.  Insol.  in  all  ordinary 
solvents.  (Miguel,  A.  ch.  (5)  11.  341.) 

Barium  sulphocyanide,  Ba(SCN)2+2H2O. 

Deliquescent.  Easily  sol.  in  H2O  and 
alcohol.  Boiling  solution  in  alcohol  contains 
32.8%  anhydrous  salt.  Solution  sat.  at  20' 
contains  30%.  (Tscherniak,  B.  16.  349.) 

Cryst.  with  3H2O.  (Tscherniak,  B.  25. 
2627.) 

Barium  cadmium  sulphocyanide, 

4Ba(SCN)2,  Cd(SCN)2+10H2O. 
Deliquescent.     (Grossmann.  B.   1902,   36 
2669.) 


Barium  caesium  cuprous  sulphocyanide, 

Ba(SCN)2,  3CsSCN,  2CuSCN. 
Rapidly  decomp.  by  H2O.     (Wells,  Am. 
Ch.  J.  1902,  28.  273.) 

Barium  caesium  silver  sulphocyanide, 
Ba(SCN)2,  3CsSCN,  2AgSCN. 

100  pts.  H2O  dissolve  92  pts.  at  19°. 

Decomp.  by  much  H2O.    (Wells,  Am.  Ch. 
J.  1902,  28.  272.) 

Barium  cobaltous  sulphocyanide, 

BaCo(SCN)4+8H2O. 


290 


Ppt.      (Rosenheim,    Z.    anorg.    1901,    27. 
0.) 


Barium  mercuric  sulphocyanide. 

BaHg(SCN)4. 

Very  sol.  in  H2O  and  in  alcohol.  (Rosen- 
heim, Z.  anorg.  1901,  27.  286.) 

BaHg(SCN)3J2+2H2O.  Ppt.  Nearly  in- 
sol.  in  cold;  easily  sol.  in  hot  H2O.  (Rosen- 
heim.) 

Barium  potassium  silver  sulphocyanide, 

Ba(SCN)2,  4KSCN,  2AgSCN+H2O. 
Very  sol.  in  a  little  H2O.     Decomp.  by 
much  H2O.     (Wells,  Am.  Ch.  J.  1902,  28. 

283.) 

Barium  rubidium  silver  sulphocyanide, 

.  BaRb2Ag2(SCN)6+2H2O. 

Very  sol.  in  H2O.  (Wells,  Am.  Ch.  J. 
1903,  30.  186.) 

BaRb4Ag2(SCN)8+H20.  Sol.  in  H20. 
(Wells.) 

Barium  silver  sulphocyanide,  Ba(SCN)2, 

2AgSC.N  +2H2O. 
Stable  in   the  air.      (Wells,   Am.   Ch.   J. 

1902,  28.  269.) 

Barium  zinc  sulphocyanide,  BaZn(SCN)4 

+3H2O. 

Easily  sol.  in  alcohol.  (Walden,  Z.  anorg. 
1900,  23.  374.) 

Barium  sulphocyanide  mercuric  bromide. 

Ba(SCN)2,  2HgBr2+5H20. 
Very  sol.  in  H2O.     (Grossmann,  Z.  anorg. 

1903,  37.  420.) 

Bismuth  sulphocyanide,  basic, 
Bi(OH)(SCN)2+5H20. 

(Rosenheim  and  Vogelgesang,  Z.  anorg. 
1906,  48.  214.) 

Bi(SCN)3,  2Bi2O3.  Insol.  in  H2O,  but 
when  recently  pptd.  decomp.  by  boiling 
therewith.  Insol.  in  HSCN+Aq.  (Meitzen- 
dorf.) 

Bismuth  sulphocyanide,  Bi(SCN)3. 

Insol.  or  si.  sol.  in  H2O.  Sol.  in  HNO8, 
HC1,  and  HSCN+Aq.  (Meitzendorf,  Pogg. 
56.  83.) 


878 


SULPHOCYANIDE,  BISMUTH  POTASSIUM 


Decomp.  by  cold  H2O.  (Bender,  B.  20 
723.) 

+  14H2O.    Extremely  deliquescent. 

Decomp.  by  H2O.  (Rosenheim  and  Vogel- 
gesang,  Z.  anorg.  1906,  48.  214.) 

Bismuth  potassium  sulphocyanide, 

K3Bi(SCN)6. 

Decomp.  by  H2O.  (Rosenheim  and  Vogel- 
gesang,  Z.  anorg.  1906,  48.  215.) 

Not  hydroscopic. 

Decomp.  by  H2O. 

Easily  sol.  in  alcohol.  (Vanino,  Z.  anorg. 
1901,  28.  220.) 

BiCSCN),.    9KSCN.      Very    hydroscopic. 

Decomp.  by  H2O. 

Sol.  in  alcohol.  (Vanino,  Z.  anorg.  1901, 
28.  221.) 

Bismuth  sodium  sulphocyanide, 

Na3Bi(SCN)6. 

As  K  salt.  (Rosenheim  and  Vogelgesang, 
Z.  anorg.  1906,  48.  215.) 

Boron  sulphocyanide,  B(SCN)3. 

Sol.  in  benzene  and  ether.  (Cocksedge, 
Chem.  Soc.  1908,  (2)  93.  217.) 

Cadmium  sulphocyanide,  Cd(SCN)2. 

SI.  sol.  in  H2O.  Sol.  in  NH4OH+Aq  with 
combination. 

Cadmium  caesium  sulphocyanide, 

CsCd(SCN)3. 

Recryst.  from  H2O.  (Wells,  Am.  Ch.  J. 
1903,  30.  148.) 

Cs4Cd(SCN)6+2H20.  Very  sol.  in  H2O. 
Can  be  recryst.  from  cone,  solution  but  de- 
comp.  on  dilution  to  CsCd(SCN)3.  (Wells.) 

Cadmium  caesium  silver  sulphocyanide, 

Cs2CdAg2(SCN)6. 
(Wells.) 

+2H20.    (Wells.) 
Cs2CdAg4(SCN)8+2H2O.    (Wells.) 
Cs4Cd3Ag,o(SCN)20+6H2O.    (Wells.) 

Cadmium  mercuric  sulphocyanide,  Cd(SCN)2, 

Hg(SCN)2. 

Very  sol.  in  hot  H2O.  (Grossmann,  Z. 
anorg.  1903,  37.  414.) 

Cadmium   molybdenum   sulphocyanide, 

Cd(SCN)2,  Mo(SCN)4+2H2O. 
(Maas  and  Sand,  B.  1908,  41.  1513.) 
+3H2O.    (Maas  and  Sand.) 

Cadmium    molybdenyl    potassium    sulpho- 
cyanide, KSCN,  4Cd(SCN)2, 
3Mo(OH)(SCN)3+18H2O. 
(Mass  and  Sand,  B.  1908,  41.  1513.) 


Cadmium  molybdenyl  sulphocyanide  am- 
monia, 3Cd(SCN)2,  2Mo(OH)(SCN)3, 
13NH3. 

(Mass  and  Sand,  B.  1908,  41.  1512.) 
+2H2O.    (Maas  and  Sand.) 

Cadmium  potassium  sulphocyanide, 

K2Cd(SCN)4+2H2O. 
Very  sol.  in  H2O.     (Grossmann,  B.  1902, 

36.  2668.) 

Cadmium  rubidium  sulphocyanide, 

Rb2Cd(SCN)4+2H2O. 
Very  sol.  in  H2O.     (Grossmann,  B.  1902, 
35.  2668.) 

Cadmium  sodium  sulphocyanide, 

NaCd(SCN)3+3H2O. 
(Grossmann,  B.  1902,  36.  2668.) 

Cadmium  sulphocyanide  ammonia,  Cd(SCN)2, 
NH3. 

Decomp.  by  H2O.  (Grossmann,  B.  1902, 
35.  2666.) 

Cd(SCN)2,  2NH3.  Decomp.  by  pure  H2O. 
(Grossmann.) 

Cadmium  sulphocyanide  ammonium  bromide, 

Cd(SCN)2,  NH4Br+H2O. 
Can  be  recryst.  from  H2O.     Decomp.  in 
dil.  solution.     (Grossmann,  Z.  anorg.  1903, 

37.  425.) 

Cd(SCN)2,  2NH4Br.  Easily  splits  off 
NH4Br.  (Grossmann.) 

Cadmium  sulphocyanide  ammonium  chloride, 

Cd(SCN)2,  2NH4C1. 

Can  be  recryst  from  H2O.  Decomp.  in  dil. 
solution.  (Grossmann,  Z.  anorg.  1903,  37. 
423.) 

Cadmium  sulphocyanide  potassium  bromide, 
Cd(SCN)2,  KBr+H2O. 

Recryst.  from  H2O.  (Grossmann,  Z.  anorg. 
1903,  37.  425.) 

Cd(SCN)2,  2KBr.  Recryst.  from  H2O. 
(Grossmann.) 

Cadmium  sulphocyanide  potassium  chloride, 

Cd(SCN)2,  2KC1. 

Recryst.  from  H2O.  Decomp.  in  dil.  solu- 
tion. (Grossmann,  Z.  anorg.  1903,  37.  423.) 

phocyank 
Cd(SCN)2,  2KI. 
Recryst.  from  H2O.    (Grossmann.) 

Caesium   calcium   silver   sulphocyanide, 

2CsSCN,  Ca(SCN)2,  2AgSCN+2H2O. 
Recryst.  from  H2O.     (Wells,  Am.  Ch.  J. 
1902,  28.  275.) 


SULPHOCYANIDE,  COBALTOUS  MERCURIC 


879 


Caesium  chromium  sulphocyanide. 
See  Chromisulphocyanide,  caesium. 

Caesium  cobaltous  sulphocyanide, 

Cs2Co(SCN)4+2H2O. 
Stable  in  the  air.     (Shinn  and  Wells,  Am. 
Ch.  J.  1903,  29.  476.) 

Caesium  cobaltous  silver  sulphocyanide, 

Cs2CoAg2(SCN)6+2H2O. 
Slowly  attacked  by  H2O;  decomp.  by  boil- 
ing H2O.    Very  si.  sol.  in  CsSCN  or  Co(SCN)2 
+Aq.     (Shinn  and  Wells,  Am.  Ch.  J.  1903, 
29.  478.) 

Caesium    cuprous     sulphocyanide,    CsSCN. 

CuSCN 

H20  separates  CuSCN.  (Roberts,  Am.  Ch. 
J.  1902,  28.  262.) 

Caesium  cuprous  nickel  sulphocyanide, 

2CsSCN,  Ni(SCN)2,  2CuSCN+2H2O. 
SI.  sol.  in  H2O.    (Roberts  and  Wells,  Am. 
Ch.  J.  1902,  28.  277.) 

Caesium   cuprous    strontium    sulphocyanide, 

3CsSCN,  2CuSCN,  Sr(SCN)2. 
As  Ba  salt.     (Wells,  Am.  Ch.  J.  1902,  28. 

275.) 

Caesium    magnesium    silver    sulphocyanide, 
2CsSCN,  Mg(SCN)2,  2AgSCN  +2H2O. 
As  Ca  comp.    (Wells,  Am.  Ch.  J.  1902,  28. 

275.) 

Caesium    manganous    silver    sulphocyanide, 

Cs2MnAg2(SCN)6+2H20. 
Rather  si.  sol.  in  H2O.    (Wells.) 

Caesium    mercuric    sulphocyanide,    CsSCN, 

Hg(SCN)2. 

SI.  sol.  in  hot  H2O.  (Bristol  and  Wells, 
Am.  Ch.  J.  1902,  28.  260.) 

Caesium  mercuric   sulphocyanide,   2CsSCN, 
Hg(SCN)2+H20. 

Moderately  sol.  in  H2O,  especially  when 
warm.  Recryst.  without  decomp.  (Bristol 
and  Wells,  Am.  Ch.  J.  1902,  28.  260.) 

Caesium  nickel  silver  sulphocyanide, 

Cs2NiAg2(SCN)6+2H2O. 
Slowly  decomp.  by  hot  H2O.    (Wells,  Am. 
Ch.  J.  1902,  28.  277.) 

Caesium      silver      sulphocyanide,     CsSCN, 
AgSCN. 

Easily  forms  supersat. .  solution.     (Wells, 
Am.  Ch.  J.  1902,  28.  264.) 
^  2CsSCN,    AgSCN.       Stable   in   the    air. 
(Wells.) 

3CsSCN,  AgSCN.  Stable  in  the  air. 
(Wells.) 


Caesium     silver     strontium     sulphocyanide, 

3CsSCN,  2AgSCN,  Sr(SCN)2. 
As  Ba  comp.    (Wells.) 

Caesium  silver  zinc  sulphocyanide, 

CsZnAg(SCN)4+H2O. 

(Wells.) 

Cs2ZnAg(SCN)6.  Ppt.  Stable  in  the  air. 
(Wells.) 

CsZn2Ag3(SCN)8.  Decomp.  by  cold,  more 
rapidly  by  hot  H2O.  (Wells.) 

CsZn2Ag4(SCN)9.  Slowly  decomp.  by 
H2O.  (Wells.) 

Caesium  zinc  sulphocyanide,  Cs2Zn(SCN)4+ 

2H2O. 

Moderately  sol.  in  H20  and  can  be  recryst. 
therefrom.  (Wells.) 

Calcium  sulphocyanide,  Ca(SCN)2+3H2O. 

Deliquescent.  Very  sol.  in  H2O  and  al- 
cohol. 

Calcium    silver    sulphocyanide,    Ca(SCN)2, 

2AgSCN+2H2O. 
(Wells.) 

Calcium  stannic  sulphocyanide,  CaSn(SCN)6 

+7H2O. 

Very  sol.  in  H2O.  Can  be  recryst.  there- 
from. Sol.  in  alcohol  and  acetone.  (Wein- 
land  and  Barnes,  Z.  anorg.  1909,  62.  258.) 

Cerous  sulphocyanide,  Ce(SCN)3+7H2O. 

Deliquescent.  Sol.  in  H2O  and  alcohol. 
(Jolin,  Bull.  Soc.  (2)  21.  534.) 

Chromous  sulphocyanide  with  MSCN. 
See  Chromosulphocyanide,  M. 

Chromic  sulphocyanide,  Cr(SCN)3. 

Deliquescent,  and  sol.  in  H2O. 

Somewhat  sol.  in  organic  solvents.  (Sper- 
ansky,  C.  C.  1897,  I.  141. 

See  also  Chromisulphocyanhydric  acid. 

Chromic  sulphocyanide  with  MSCN. 
See  Chromisulphocyanide,  M. 

Cobaltous  sulphocyanide,  Co(SCN)2+^H2O. 

Sol.  in  H2O  and  alcohol;  also  in  ether.  Sol. 
in  liquid  SO2.  (Walden,  B.  1899,  32.  2864.) 

Sol.  in  acetone.    (Krug  and  M'Elroy.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

+3H2O.  Sol.  in  H2O  and  in  alcohol. 
(Rosenheim  and  Cohn.  Z.  anorg.  1901,  27. 
288.) 

Cobaltous  mercuric  sulphocyanide,  Co(SCN)2. 

Hg(SCN)2. 

Very  si.  sol.  in  H2O  and  dil.  HCl+Aq. 
Easily  sol.  in  HNO3+Aq.  (Cleve,  J.  pr.  91. 

227.) 


880 


SULPHOCYANIDE,  COBALTOUS  POTASSIUM 


Cobaltous  potassium  sulphocyanide, 

CoK2(SCN)4. 

Decomp.  by  H2O.  (Treadwell,  Z.  anorg. 
1901,  26.  109.) 

+4H2O.  Sol.  in  H2O.  Sol.  in  methyl, 
ethyl  and  amyl  alcohol,  in  acetone  and  in 
ether +Aq.  Can  be  recryst.  from  H2O  or 
alcohol  without  decomp.  (Rosenheim  and 
Cohn,  Z.  anorg.  1901,  27.  289.) 

Cobaltous  silver  sulphocyanide,  CoAg(SCN)3 
+2H2O. 

Decomp.  by  H2O.  (Shinn  and  Wells,  Am. 
Ch.  J.  1903,  29.  476.) 

Ag2Co(SCN)4.  Almost  insol.  in  H2O  and 
in  alcohol.  (Rosenheim,  Z.  anorg.  1901,  27. 
291.) 

Cobaltous  sodium  sulphocyanide, 

Na2Co(SCN)4+8H2O. 
Sol.  in  H2O  and  in  alcohol.    (Rosenheim.) 

Cobaltous  sulphocyanideammonia,Co(SCN)2/ 
2NH3  and  Co(SCiV;2,  6NH3. 

(Peters,  B.  1908,  41.  3178.) 

Co(SCN)2,  4NH3.  Sol.  in  H2O  and  alcohol. 
(Sand,  B.  1903,  36.  1439.) 


Cobaltous  sulphocyanide  mercuric  chloride. 

2Co(SCN)2,  2HgCl2. 

(Hantzsch  and  Shibata.  Z.  anorg.  1912,  73. 
320.) 

2Co(SCN)2,  3HgCl2.  Easily  decomp. 
(Hantsch  and  Shibata.) 

Cuprous  sulphocyanide,  CuSCN. 

1  1.  H2O  at  18°  dissolves  0.004  mg.  mols. 
or  0.5  mg.  CuSCN.  (Kohlrausch  and  Rose, 
Z.  phys.  Ch.  1893,  12.  241.) 

Insol.  in  dil.  acids.  SI.  sol.  in  cold,  easily 
in  warm  cone.  HCl+Aq.  Decomp.  by  cone. 
H2SO4  or  HNO3+Aq.  Sol.  with  combination 
in  NH4OH+Aq.  Insol.  in  KSCN+Aq. 

Less  sol.  in  H2SO3  and  H2SO4+Aq  than  in 
HNO3.  (Kuhn,  Ch.  Z.  1908,  32.  1056.) 

Sol.  in  Fe2(SO4)3+Aq.  (Johnson,  J.  Soc. 
Chem.  Ind.  1889,  8.  603.) 

KSCN+Aq  (85-90  g.  in  50  g.  H2O)  dis- 
solves 18  g.  CuSCN.  (Thurnauer,  B.  1890, 
23.  770.) 

Sol.  in  ether.    (Skey,  C.  N.  1867,  16.  201.) 

Cupric  sulphocyanide,  Cu(SCN)2. 

Decomp.  by  H2O  to  cuprous  salt.  Sol.  in 
warm  HC1,  H2SO4,  or  HNO3+Aq.  Sol.  in 
MSCN+Aq,  but  solutions  decomp.  by  dilu- 
tion. Sol.  in  NH4OH+Aq. 


Solubility  in  NH4OH+Aq  at  25°  and  at  40°. 
At  25°. 


One  gram  of  solution  contains 

1000  mols.  H2O  dissolve 

Composition  of  solid 

Sp.  gr.  25°/25° 

salt  in  contact  with 

g.  NH3 

g.  Cu(SCN)2 

g.  H20 

Mols.  NH3 

Mols. 

Cu(SCN)2 

solution 

0.99853 

0.2147 

0.1522 

0.6331 

358.04 

24.09 

0.99871 

0.1655 

0.1124 

0.7221 

242.02 

15.60 

.00703  . 
.01336 

0.0993 
0.0639 

0.0798 
0.0659 

0.8209 
0.8702 

127.76 
77.51 

9.74 
7.59 

•  Cu(SCN),,:4NHi 

.01506 

0.0535 

0.0622 

0.8843 

64.05 

7.04 

.01705 

0.0426 

0.0596 

0.8978 

50.21 

6.65 

.02132 

0.0250 

0.0511 

0.9239 

28.55 

5.55 

.01661 

0.0198 

0.0408 

0.9394 

22.27 

4.35 

Cu(SCN)2,  2NH3 

.00816 

0.0079 

0.0245 

0.9676 

18.61 

2.54 

At  40°. 


0.1802 

0.1976 

0.6222 

306.28 

31.83 

0.1398 

0.1658 

0.6944 

213.10 

23.93 

0.0758 
0.0550 

0.1299 
0.1207 

0.7943 
0.8243 

101.00 
70.59 

16.38 
14.67 

Cu(SCN)2,^4NH3 

0.0435 

0.1178 

0.8388 

54.82 

14.07 

0.0352 

0.0876 

0.8772 

42.53 

10.00 

0.0257 

0.0655 

0.9088 

30.00 

7.22 

0.0177 

0.0418 

0.9405 

19.86 

4.46 

>[Cu(SCN)2,  2NH3 

0.0094 

0.0281 

0.9625 

10.31 

2.93 

(Horn,  Am.  Ch.  J.  1907,  37.  471.) 


Insol.  in  methyl  acetate.     (Naumann,  B. 
1909,  42.  3790.) 


Cuprocupric  sulphocyanide,  Cu(SCN)2, 

Cu2(SCN)2. 

Not  attacked  by  hot  HCl+Aq.     Insol.  in 
KSCN+Aq. 


SULPHOCYANIDE,  LEAD,  BASIC 


881 


Cupric  mercuric  sulphocyanide,  CuHg(SCN)4. 
Almost  inspl.  in  cold  H2O  and  in  alcohol; 
si.  sol.  in  boiling  H2O.    (Rosenheim,  Z.  anorg. 
1901,  27.  286.) 

Cuprous  potassium  sulphocyanide,  CuSCN, 

6KSCN. 

Deliquescent.  Decomp.  by  H2O.  (Thurn- 
auer,  B.  1890,  23.  770.) 

Cuprous  sulphocyanide  ammonia,  Cu2(SCN)2, 
2NH3. 

Decomp.  in  the  air.  (Richards,  Z.  anorg. 
1898,  17.  247.) 

Cu2(SCN)2,  5NH3.  Very  unstable  in  the 
air.  (Richards.) 

Cupric  sulphocyanide  ammonia,  Cu(SCN)2, 
2NH3. 

Sol.  in  little  H2O,  but  decomp.  by  dilution 
with  pptn.  of  basic  salt.  Sol.  in  NH4OH+Aq. 

By  long  standing  a  small  amount  dissolves 
in  H2O  with  separation  of  CuSCN.  (Litter- 
scheid,  Arch.  Pharm.  1901,  239.  337.) 

Insol.  in  H2O.  Sol.  in  H20  containing 
a  small  amount  of  ammonia.  (Horn,  Am. 
Ch.  J.  1907,  37.  477.) 

Cu(SCN)2,  4NH3.  Very  unstable  in  the 
air. 

Sol.  in  H2O,  but  decomp.  by  much  H2O 
with  pptn.  of  a  basic  salt.  (Horn.) 

100  pts.  N/10  NH4OH+Aq  dissolve  10.4 
pts.  anhydrous  salt  at  25°.  (Pudschies,  Dis- 
sert.) 

Loses  NH3  in  the  air. 

Sol.  in  H2O.  (Kohlschiitter,  B.  1904,  37. 
1156.) 

Decomp.  in  the  air  and  by  H20  and  dil. 
and  cone,  acids;  sol.  in  cold  cone.  HNO3  and 
NH4OH+Aq.  Sol.  in  boiling  cone.  HC1. 
(Richards,  Z.  anorg.  1898, 17.  250.) 

Didymium  sulphocyanide,  Di(SCN)3+6H2O. 
Deliquescent,  and  sol.  in  H2O. 

Erbium  sulphocyanide,  Er(SCN)3+6H2O. 
Deliquescent.     Sol.  in  H2O.     (Hoglund.) 

Glucinum  sulphocyanide,  G1(SCN)2  (?). 
Sol.  in  H2O.    (Hermes,  J.  pr.  97.  465.) 

Gold  (aurous)  potassium  sulphocyanide, 

AuSCN,  KSCN. 

Easily  sol.  in  H2O,  less  in  absolute  alcohol. 
(Cleve,  J.  pr.  94.  16.) 


Gold 


ocyanide 


(aurous)    potassium    sulpho 
ammonia,  KAu(SCN)2,  5NH3. 
(Peters,  B.  1908,  41.  3178.) 


Gold   (auric)   potassium  sulphocyanide  am- 
monia, KAu(SCN)4,  4NH3. 
(Peters.) 


Gold  (aurous)  silver  sulphocyanide,  AuSCN, 

AgSCN. 
Insol.  in  H2O.     Sol.  in  NH4OH+Aq. 

Gold  (auric)  potassium  sulphocyanide. 
Sol.  in  H2O,  alcohol,  and  ether.     (Cleve.) 

Gold  (aurous)  sulphocyanide  ammonia, 

AuSCN,  NH3. 
Very  si.  sol.  in  cold,  decomp.  by  hot  H2O. 

Iron    (ferrous)    sulphocyanide,    Fe(SCN)2  + 

3H2O. 

Very  sol.  in  H2O,  alcohol,  or  ether. 
Sol.  in  acetone.    (Krug  and  M'Elroy.) 

Iron  (ferric)  sulphocyanide,  Fe(SCN)3+3H2O. 
Deliquescent.  Very  sol.  in  H2O,  alcohol, 
or  ether.  Ether  extracts  the  salt  from 
Fe(SCN)3+Aq.  Decomp.  by  much  H2O 
if  pure.  Not  decomp.  by  monobasic  acids, 
but  cone.  H2SO4,  and  H8PO4,  also  oxalic, 
tartaric,  malic,  etc.,  acids  destroy  the  colour. 

Iron  (ferric  )lithium  sulphocyanide,  Fe(SCN)«, 

9LiSCN+4H20. 

More  deliquescent  than  the  other  ferric 
sulphocyanides.  (Kriiss  and  Moraht.) 

Iron  (ferrous)  mercuric  sulphocyanide, 

Fe(SCN)2,   Hg(SCN)2+2H20. 
Moderately  sol.  in  hot  H2O.     (Cleve,  J. 
pr.  91.  227.) 

Iron   (ferric)   potassium   sulphocyanide, 
Fe(SCN)3,  3KSCN+zH2O. 

Extremely  deliquescent,  and  sol.  in  H2O. 
(Kriiss  and  Moraht.) 

Fe(SCN)3,  9KSCN+4H2O.  Hygroscopic. 
Sol.  in  H2O  without  decomp.  Insol.  in  pure 
anhydrous  ether,  but  decomp.  by  ether  con- 
taining traces  of  H2O  into  Fe(SCN)3  and 
KSCN.  (Kriiss  and  Moraht,  A.  260.  204.) 

Iron  (ferrous)  sodium  sulphocyanide, 

Na4Fe(SCN)6+12H2O. 
Sol.  in  H2O  and  alcohol.     (Rosenheim,  Z. 
anorg.  1901,  27.  299.) 

Iron  (ferric)  sodium  sulphocyanide,  Fe(SCN)s, 
9NaSCN+4H20. 

Less  deliquescent  than  the  corresponding 
NH4  or  K  salt.  (Kriiss  and  Moraht.) 

Na3Fe(SCN)6+12H2O.  (Rosenheim,  Z. 
anorg.  1901,  27.  297.) 

Lanthanum    sulphocyanide,    La(SCN)8+ 

7H20. 
Deliquescent;  sol.  in  H2O.     (Cleve.) 

Lead  sulphocyanide,  basic, 

6PbO,  Pb(SCN)2+2H2O.    Ppt. 
Pb(SCN)2,    PbO+H2O.     Insol.    in   H2O. 
(Stromholm,  Z.  anorg.  1904,  38.  440.) 


882 


SULPHOCYANIDE,  LEAD 


Lead  sulphocyanide,  Pb(SCN)2. 

Nearly  insol.  in  cold,  decomp.  by  boiling 
H2O.  (Liebig.) 

SI.  sol.  in  H2O. 

4.5X10  -1  g.  are  dissolved  in  1  liter  of  sat. 
solution  at  20°.  (Bottger,  Z.  phys.  Ch.  1903, 
46.  603.) 

Lead    sulphocyanide    bromide,    Pb(SCN)2, 

8PbBr2. 
(Grissom  and  Thorp,  Am.  Ch.  J.  10.  219.) 

Lead  sulphocyanide  chloride,  PbSCNCl. 

SI.  sol.  in  cold,  easily  sol.  in  hot  H2O. 
(Murtry,  Chem.  Soc.  55.  50.) 

Sol.  in  H2O.  (Grissom  and  Thorp,  Am. 
Ch.  J.  10.  229.) 

Lead  sulphocyanide  iodide,  3Pb(SCN)2,  PbI2. 
Sol.  in  H2O.     (Grissom  and  Thorp,  Am. 
Ch.  J.  10.  229.) 

Lithium  sulphocyanide,  LiSCN. 

Very  deliquescent.  Sol.  in  H2O  and  alco- 
hol. (Hermes,  Z.  Ch.  1866.  417.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3789.) 

Magnesium   sulphocyanide,    Mg(SCN)2  + 

4H2O. 

Deliquescent.  Easily  sol.  in  H2O  and 
alcohol. 

Magnesium  stannic  sulphocyanide, 

MgSn(SCN)6+6H2O. 

Hygroscopic.  Sol.  in  H2O,  alcohol  and 
acetone.  (Weinland  and  Barnes,  Z.  anorg. 
1909,  62.  258.) 

Manganous     sulphocyanide,     Mn(SCN)2  + 

3H20. 

Deliquescent.  Easily  sol.  in  H2O  and 
alcohol. 

Mercurous   sulphocyanide,   Hg2(SCN)2. 

Insol.  in  H2O.  Sol.  in  hot  HCl+Aq. 
Slowly  decomp.  by  hot  aqua  regia.  Sol.  in 
hot  KSCN+Aq. 

Mercuric  sulphocyanide,  basic,  Hg(SCN)2, 
3HgO. 

Insol.  in  H2O.  Easily  sol.  in  HCl+Aq. 
Insol.  in  H2SO4  or  HN03+Aq.  (Fleischer.) 

Hg(SCN)2,  2HgO.  Insol.  in  H2O.  SI. 
attacked  by  acids.  (Glaus,  J.  pr.  15.  401.) 

Mercuric  sulphocyanide,  Hg(SCN)2. 

Very  si.  sol.  in  cold,  much  more  easily  in 
hot  H2O.  Easily  sol.  in  dil.  HCl+Aq. 
(Crookes,  Chem.  Soc.  4.  18.) 

Solubility  in  H2O=  0.00218  mol.  in  1  1. 
(Grossmann,  Z.  anorg,  1904,  43.  358.) 

More  sol.  in  H2O  than  in  alcohol.  (Peters, 
B.  1908,  41.  3180.) 


Very  si.  sol.  in  H2O  at  25°.  Appreciably 
sol.  only  in  boiling  H2O.  (Jander  Dissert. 
1902.) 

Sol.  in  Hg(NO3)2  or  KSCN+Aq,  also  in 
NH4Cl+Aq.  Sol.  in  many  sulpho cyanides 
+Aq. 

Easily  sol.  in  cold  HC1,  NH4C1,  KC1  or 
BaCl2+Aq.  (Hermes,  J.  pr.  1866,  (1)  97. 
477.) 

Very  sol.  in  liquid  I\H3.  (Franklin,  Am. 
Ch.  J.  1898,  20.  829.) 

SI.  sol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1369.) 

Mercuric  hydrogen  sulphocyanide, 

Hg(SCN)2,  2HSCN. 
.  Easily  decomp.     (Hermes,    Dissert.  1866.) 

Mercuric  nickel  sulphocyanide,  Hg(SCN)2, 
Ni(SCN)2+2H2O. 

Moderately  sol.  in  hot  H2O.  (Cleve,  J. 
pr.  91. 227.) 

Very  sol.  in  MSCN+Aq.  (Orloff,  C.  C. 
1906,  I.  1411.) 

Mercuric   potassium   sulphocyanide, 
Hg(SCN)2,  KSCN. 

Sol.  in  cold,  more  easily  in  hot  H2O.  Sol. 
in  alcohol  and  ether.  Very  sol.  in  NH4C1  or 
KCl+Aq.  (Glaus.) 

K2Hg(SCN)4.  Very  sol.  in  H2O;  sol.  in 
alcohol. 

Insol.  in  anhydrous  ether.  (Rosenheim, 
Z.  anorg.  1901,  27.  285.) 

Mei  curie  rubidium  sulphocyanide, 
Hg(SCN)2,  RbSCN. 

Sol.  in  alcohol  without  decomp.  Decomp. 
by  H2O. 

Hg(SCN)2,  2RbSCN  +  ^H2O.  Easily  sol. 
in  H2O  without  decomp.  (Grossmann,  B. 
1904,  37.  1259.) 

Mercuric  sodium  sulphocyanide, 

Na2Hg(SCN)3. 

Very  hydroscopic.  (Rosenheim,  Z.  anorg. 
1901,  27. 286.) 

Mercuric    zinc    sulphocyanide,    Hg(SCN)2, 

Zn(SCN)2. 

Scarcely  sol.  in  cold  H2O.  Easily  sol.  in 
HCl+Aq.  (Cleve.) 

Mercuric  sulphocyanide  ammonia, 

2Hg(SCN)2,  3NH3+^H20. 
Decomp.  by  H2O  and  alcohol. 
Hg(SCN)2,   4NH3.     (Peters,  B.    1908,  41. 
3178.) 

Mercuric  sulphocyanide  ammonium  bromide, 

Hg(SCN)2,  NH4Br. 

Decomp.  by  H2O.  Sol.  in  alcohol.  (Gross- 
mann, Z.  anorg.  1903,  37.  418.) 


SULPHOCYANIDE,  POTASSIUM 


883 


Mercuric  sulphocyanide  ammonium  chloride 

Hg(SCN)2,  NH4C1. 

Deocmp.  by  H2O.  Sol.  in  warm  alcoho 
from  which  it  can  be  cryst.  (Grossmann.) 

Mercuric  sulphocyanide  bromide,  HgSCNBr 

Insol.  in  cold  H2O;  sol.  in  hot  H2O  and  in 

alcohol.      (Rosenheim,   Z.   anorg.    1901,   27. 

282.) 

Mercuric  sulphocyanide  chloride,  HgSCNCl. 
Insol.  in  cold  H2O. 
Sol.  in  hot  H2O  and  alcohol.    (Rosenheim.) 

Mercuric  sulphocyanide  potassium  bromide, 

Hg(SCN)2,  2KBr. 
Very  sol.  in  H2O.     (Grossmann,  Z.  anorg. 
1903,  37.  418.) 

Mercuric  sulphocyanide  potassium  chloride, 
Hg(SCN)2,  KC1. 

Decomp.  by  H2O. 

Not  decomp.  by  recryst.  from  warm  alcohol 
(Grossmann.) 

Molybdenum  sulphocyanide,  Mo(SCN)3(?). 

Sol.  in  H2O  and  ether.  (Braun,  Z.  anal.  6. 
86.) 

Molybdenum  potassium  sulphocyanide, 

K3Mo(SCN)6+4H2O. 
Cryst.  from  boiling  H2O  and  alcohol. 
(Chilesotti,  Gazz.  ch.  it.  1904,  34.  (2)  493.) 

Molybdenum  sodium  sulphocyanide, 

Na3Mo(SCN)6  +  12H2O. 
(Rosenheim,  B.  1909,  42.  154.) 

Molybdenum  thallous  sulphocyanide, 

MoTl3(SCN-)6. 
(Rosenheim  and  Garfunkel,  B.  1908,  41. 

2388.) 

Molybdenum  sulphocyanide  zinc  amine, 

2Mo(SCN)6,  3Zn(NH3)4. 

(Rosenheim  and  Garfunkel,  B.  1908,  41. 
2390.) 

2Mo(SCN)6(OH),  Zn,(NH8)n.  Can  be 
cryst.  from  boiling  NH4OH+Aq.  Air-dried 
salt  probably  has  the  composition 
2Mo(SCN)6  (OH),  3Zn(NH3)4+2H20.  (Maas 
and  Sand,  B.  1908,  41.  1510.) 

2Mo(SCN)6(OH),  Zn3(NH3)I3.  (Maas  and 
Sand.) 

Nickel  sulphocyanide,  Ni(SCN)2. 

Sol.  in  H2O.  (Grossmann,  B.  1904,  37. 
565.) 

+  ^H2O.  Sol.  in  H2O  and  alcohol.  Insol. 
in  acetone.  (Krug  and  M'Elroy.) 

+1^H2O.  Sol.  in  H2O.  (Rosenheim 
and  Cohn,  Z.  anorg.  1901,  27.  292.) 


Nickel  potassium  sulphocyanide, 
K4Ni(SCN)6+4H20. 

Sol.  in  H2O  with  decomp. 

SI.  sol.  in  cold,  easily  sol.  in  hot  alcohol. 
(Rosenheim,  Z.  anorg.  1901,  27.  292.) 

Nickel  sodium  sulphocyanide, 

NiNa2(SCN)4+8H2O. 
Sol.  in  H2O  with  decomp. 
SI.   sol.   cold,   readily  sol.   hot  alcohol. 
(Rosenheim,  Z.  anorg.  1901,  27.  292.) 

Nickel  sulphocyanide  ammonia,   Ni(SCN)2, 

3NH3. 

(Peters,  B.  1908,  41.  3178.) 
Ni(SCN),,  4NH,.     Decomp.   by  H2O. 

Platinous  sulphocyanide,  Pt(SCN)2(?). 

Insol.  in  H2O. 

See  Platinosulphocyanides,  and  Platmoso- 
sulphocyanides. 

Potassium  sulphocyanide,  KSCN. 

Deliquescent.  Very  sol.  in  H2O.  100 
pts.  H2O  dissolve  177.2  pts.  at  0°,  and  217.0 
pts.  at  20°. 

100  g.  sat,  KSCN+Aq  contain  70.5  g. 
KSCN  at  25°.  (Foote,  Z.  phys.  Ch.  1903,  46. 
81.) 

150  pts.  KSCN +100  pts.  H2O  at  10.8° 
lower  the  temp.  34.5°.  (Riidorff,  B.  2.  68.) 

Solubility  of  KSCN  +AgSCN  at  25°. 


% 

KSCN 

% 

AgSCN 

Solid  phase 

70.53 

0.00 

KSCN 

66.55 

9.32 

KSCN+2KSCN,  AgSCN 

64.47 

10.62 

2KSCN,  AgSCN 

61.25 

11.76 

tt 

58.34 

13.55 

(t 

53.21 

17.53 

(( 

50.68 

20.43 

2KSCN,  AgSCN  +KSCN, 
AgSCN 

49.43 

20.32 

KSCN,  AgSCN 

32.51 

18.34 

(( 

24.68 

16.41 

u 

23.86 

16.07 

KSCN,  AgSCN  +  AgSCN 

(Foote,  Z.  phys.  Ch.  1903,  46.  81.) 
See  also  AgSCN. 

Sol.  in  alcohol,  especially  easily  if  boiling. 

Sol.    in   acetone.      (Krug   and    M'Elroy.) 

Sol.  in  liquid  SO2.  (Walden,  Z.  anorg. 
1902,  30.  160.) 

100  g.  acetone  dissolve  20.75  g.  KSCN  at 
22°,  and  20.40  g.  at  58°. 

100  g.  amyl  alcohol  dissolve  0.18  g.  KSCN 
at  13°;  1.34  g.  at  65°;  2.14  g.  at  100°;  3.15  g. 
at  133.5.° 

100  g.  ethyl  acetoate  dissolve  0.44  g.  KSCN 
at  0°;  0.40  g.  at  14°;  0.20  g.  at  79°. 

100  g.  pyridine  dissolve  6.75  g.  KSCN  at 
0°;  6.15  g.  at  20°;  4.97  g.  at  58°;  3.88  g.  at 


884 


SULPHOCYANIDE,  POTASSIUM  MOLYBDENYL 


97°;  3.21  g.  at  115°.  (Laszcynski,  B.  1894, 
27.  2285.) 

100  g.  acetonitrile  dissolve  11.31  g.  KSCN 
at  18°.  (Naumann  and  Schier,  B.  1914,  47. 
249. 

SI.  sol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1369.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3789.) 

Potassium        molybdenyl        sulphocyanide, 

3KSCN,  Mo(OH)(SCN)3+4H2O. 
Sol.  in  H2O.     (Sand  and  Maas,  B.  1908, 
41.  1506.) 

Potassium     silver     sulphocyanide,     KSCN, 

AgSCN. 

Decomp.  by  H20. 
See  Donk  .under  KSCN. 
2KSCN,    AgSCN.      Stable    in    the    air. 
(Wells,  Am.  Ch.  J.  1902,  28.  265.) 
See  Donk  under  KSCN. 
3KSCN,  AgSCN.    (Wells.) 

Potassium  stannic  sulphocyanide. 

K2Sn(SCN)6+4H20. 
Very  sol.  in  H2O. 

Sol.  in  alcohol  and  acetone.  (Weinland 
and  Barnes,  Z.  anorg.  1909,  62.  258.) 

Potassium  titanyl  sulphocyanide, 
2KSCN,  TiO(SCN)2+H2O. 
Sol.  in  cold  H2O  without  immediate  de- 
comp.  but  slowly  decomp.     (Rosenheim  and 
Cohn,  Z.  anorg.  1901,  28.  169.) 

Potassium  vanadium  sulphocyanide, 
3KSCN,  V(SCN)3+4H2O. 

Sol.  in  H2O.  Sol.  in  alcohol  with  a  green 
color.  SI.  sol.  in  ether.  (Ciocci,  Z.  anorg. 
1898,  19.  309.) 

Sol.  in  H2O  with  decomp.;  stable  in  aq. 
solution  in  the  presence  of  an  excess  of  KSCN; 
sol.  in  alcohol.  (Locke,  Am.  Ch.  J.  1898,  20. 
604.) 

Potassium  vanadyl  sulphocyanide, 

K2VO(SCN)4+5H20. 
Sol.  in  H2O,  alcohol,  ether,  amyl  alcohol 
and  ethyl  acetate.     (Koppel,  Z.  anorg.  1903, 
36.  292.) 

Potassium  zinc  sulphocyanide,  2KSCN, 

Zn(SCN)2+3H2O. 

Easily  sol.  in  alcohol.  (Walden,  Z.  anorg. 
1900,  23.  374.) 

Potassium  sulphocyanide  mercuric  bromide, 
KSCN,  HgBr2. 

Very  sol.  in  H2O. 

Sol.  in  alcohol.  (Grossmann,  B.  1902, 
36.  2945.) 

2KSCN,  HgBr2.  Very  sol.  in  H2O.  Sol. 
in  alcohol.  (Grossman.) 


Potassium  sulphocyanide  mercuric  iodide, 
2KSCN,  HgI2. 

Undecomp.  by  solution  in  cone,  alcohol, 
or  in  KSCN+Aq.  (Grossmann,  Z.  anorg. 
1903,  37.  421.) 

+2H2O.  Decomp.  by  H2O.  (Philipp, 
Pogg,  1867,  131.  94.) 

Silicon  sulphocyanide,  Si(SCN)4. 

Decomp.  by  H2O  and  alcohol. 

Sol.  in  CS2,  CHC13  and  ligroin,  (Reynolds, 
Proc.  Chem.  Soc.  1906,  22.  17.) 

Silver  sulphocyanide,  AgSCN. 

1  1.  H2O  dissolves  1.08X10;6  g.  mols. 
AgSCN  at  25°.  (Kuster  and  Thiel,  Z.  anorg. 
1902,  33.  139.) 

1  1.  H2O.  dissolves  1.25X106  gram-atoms 
of  silver  at  25°.  (Abegg  and  Cox,  Z.  phys. 
Ch.  1903,  46.  11.) 

SI.  sol.  in  H2O.  1  liter  of  sat.  solution  at 
19.96°  contains  1.37  X 10  4  g.  (Bottger, 
Z.  phys.  Ch.  1903,  46.  603.) 

6.4  milligrams  are  dissolved  in  1  liter  of 
sat.  solution  at  100°.  (Bottger,  Z.  phys.  Ch. 
1906,  56.  93.) 

Solubility  product  of  AgSCN  is  0.49  and 
1.16X10-12  mols.  per  1.  at  18°  and  25°  re- 
spectively. (Kirschner,  Z.  phys.  Ch.  1912, 
79.  245.) 

Solubility  in  H2O  =  1.2X10-°  g.  mol.  per 
liter  at  25°.  (A.  E.  Hill,  J.  Am.  Chem.  Soc. 
1908,  30.  74.) 

1  1.  H2O  dissolves  0.00025  g.  AgSCN  at 
21°.  (Whitby,  Z.  anorg.  1910,  67.  108.) 

Insol.  in  acids,  excepting  cone.  H2SO4  or 
HNO3.  Insol.  in  dil.,  sol.  in  cone.  NH4OH  + 
Aq.  Sol.  in  KSCN+Aq.  Insol.  in  AgNO3 
or  NH4SCN+Aq.  Sol.  in  Hg2(NO3)2  + 
Aq. 

Solubility  in  KSCN  at  25°. 


Mol.  KSCN  in  1  litre 

g.  AgSCN  in  1 

litre 

1.25 
1.20 
1.12 
1.066 
0.626 
0.573 

22.34 
19.93 
16.18 
14.10 
2.80 
2.06 

(Hellwig,  Z.  anorg.  1900,  25.  184. 


Solubility  in  N/10  KSON+Aq  at  18°  =  2.5 
X10  4.  (Kirschner,  Z.  phys.  Ch.  1912,  79. 
247.) 

See  also  KSCN. 

1  1.  of  a  3-N  solution  of  AgNO3  dissolves 
0.432  g.  AgSCN  at  25°.  Nearly  insol.  in  less 
dil.  solution.  (Hellwig,  Z.  anorg.  1900,  25. 
179.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Insol.  in  ethyl  acetate.  (Hamers,  Dissert. 
1906;  Naumann,  B.  1910,  43.  314.) 


SULPHOCYANIDE,  TIN 


885 


Silver    strontium    sulphocyanide,    2AgSCN, 

Sr(SCN)2+2H2O. 

Stable  in  the  air.  (Wells,  Am.  Ch.  J.  1902, 
28.  270.) 

Silver       zinc        sulphocyanide,       2AgSCN, 

Zn(SCN)2. 
Decomp.  by  hot  H2O.    (Wells.) 

Silver     sulphocyanide     ammonia,     AgSCN, 

2NH3. 
Decomp.  by  H2O. 

Samarium  sulphocyanide,  Sm(SCN)3+6H2O. 
Very  deliquescent.    (Cleve.) 

Sodium  sulphocyanide,  NaSCN. 

Very  deliquescent.  Very  sol.  in  H2O  and 
alcohol. 

Sol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1369.) 

Sol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3789.) 

Sodium  stannic  sulphocyanide,  Na2Sn(SCN)6 

+6H2O. 

Very  sol.  in  H2O.  Sol.  in  alcohol  and  ace- 
tone. (Weinland  and  Barnes,  Z.  anorg.  1909, 
62.  257.) 

Sodium  vanadium  sulphocyanide,  3NaSCN, 

V(SCN)3  +  12H2O. 

Very  hygroscopic.  Sol.  in  H2O  and  alcohol. 
(Ciocci,  Z.  anorg.  1898,  19.  313.) 

Strontium  sulphocyanide,  Sr(SCN)2+3H2O. 

Very  deliquescent,  and  sol.  in  H2O  and 
alcohol. 

Strontium  stannic  sulphocyanide,  SrSn(SCN)6 

+  12H2O. 

Sol.  in  H2O,  alcohol  and  acetone.  (Wein- 
land and  Barnes,  Z.  anorg.  1909,  62.  259.) 

Thallium  sulphocyanide,  T1SCN. 

SI.  sol.  in  H2O.  3.15  g.  are  contained  in 
1  liter  of  sat.  solution  at  20°;  3.905  g.  at  25°; 
7.269  g.  at  39.75°.  Insol.  in  alcohol.  (Bott- 
ger,  Z.  phys.  Ch.  1903,  46.  603.) 

Titanyl  sulphocyanide,  TiO(SCN)2+2H2O. 
Sol.  in  cold  H2O. 

Tin  (stannous)  sulphocyanide,  Sn(SCN)2. 

Sol.  in  H20  and  alcohol.  (Classen,  J.  pr.  96. 
349.) 

Sol.  in  cold  H20.  (Rosenheim,  Z.  anorg. 
1901,  28.  168.) 

Yttrium  sulphocyanide,  Y(SCN)3+6H2O. 

Not  deliquescent.  Very  sol.  in  H2O,  al- 
cohol, or  ether. 


Zinc  sulphocyanide,  Zn(SCN)2. 

Less  sol.  in  H2O  and  alcohol  than  most  other 
cyanides. 

Zinc    sulphocyanide    ammonia.     Zn(SCN)2, 

12NH3. 
Decomp.  by  H2O.    Sol.  in  NH4OH+Aq. 

Sulphocyanoplatinic  acid. 
See  Platinosulphocyanhydric  acid. 

Sulphocyanoplatinous  acid. 
See  Platinososulphocyanhydric  acid. 

Sulphohypophosphoric  acid. 

Aluminum  sulphohypophpsphate,  A12(PS3)3. 

Unstable  in  the  air.  Sol.  in  H2O  with  de- 
comp.  (Friedel,  C.  R.  1894,  119.  262.) 

Cadmium  — ,  Cd2P2S6. 

Partially  decomp.  in  moist  air.  Decomp. 
by  H2O,  cold  HNO3  or  alkalis +Aq.  (Fer- 
rand,  A.  ch.  1899,  (7)  17.  423;  Bull.  Soc.  1895, 
(3)  13.  116.) 

Chromium  — — ,  Cr2P2S6. 

Insol.  in  HNO3.  Very  si.  attacked  by  aqua 
regia.  (Ferrand.) 

Cupric  — ,  Cu2P2S6. 

Ppt.    (Friedel,  C.  R.  1894,  119.  262.) 

Iron  (ferrous)  — — •,  Fe2P2S6. 

Sol.  in  HNO3  and  in  a  mixture  of  HNO3 
with  KC1O3.  (Friedel.) 

Lead  — ,  Pb2P2S6. 

Not  decomp.  by  boiling  H2O.    (Friedel.) 

Mercuric  — — ,  Hg2P2S6. 

Slowly  decomp.  by  boiling  H2O,  more 
rapidly  by  KOH+Aq.  (Friedel.) 

Nickel  — ,  Ni2P2S6. 

Not  attacked  by  boiling  H2O  or  hot  or  cold 
acids.  SI.  attacked  by  aqua  regia.  (Ferrand. 
A.  ch.  1899,  (7)  17.  416.) 

Silver •,  Ag4P2S6. 

Ppt.    (Friedel,  C.  R.  1894,  119.  263.) 

Tin  (stannous)  hypophosphate  — • — ,  SnPS3. 

Decomp.  by  boiling  H2O.  Sol.  in  dil.  KOH 
+Aq.  (Friedel,  C.  R.  1894,  119.  264.) 

Tin  (stannic)  — ,  SnP2S6. 

Easily  decomp.  by  boiling  H2O.  Sol.  in 
dil.  KOH+Aq.  (Friedel.) 


SULPHOHYPOPHOSPHATE,  ZINC 


Zinc  sulphohypophosphate,  Zn2P2S6. 

Decomp.  in  moist  air.  Insol.  in  H2O.  Par- 
tially decomp.  by  boiling  H2O.  Violently 
attacked  by  HNO3.  Sol.  in  aqua  regia.  Not 
attacked  by  HC1.  (Ferrand,  A.  ch.  1899, 
(7)  17.  421.) 

Zinc ,  Zn2P2S6. 

Insol.  in  H2O.  Partly  decomp.  by  boiling 
H2O.  Not  decomp.  by  HC1  or  HNO3  but  by 
aqua  regia.  (Ferrand,  Bull.  Soc.  1895,  (3)  13. 
115.) 

Sulphomolybdic  acid. 

Ammonium  sulphcmolybdate,  (NH4)2MoS4. 

Easily  sol.  in  H2O;  very  si.  sol.  in  alcohol. 
(Berzelius,  Pogg.  83.  261.) 

Ammonium  cupric  sulphomolybdate. 

SI.  sol.  in  H2O.    (Debray,  C.  R.  96.  1616.) 

Barium  sulphomolybdate,  BaMoS4. 

More  sol.  in  H2O  than  BaMo3Si0.  Known 
only  in  solution.  (Berzelius.) 

BaS,  3MoS3=BaMo3Si0.  SI.  sol.  in  cold, 
easily  sol.  in  hot  H2O.  Not  decomp.  by  cone 


'L 


cold   HNO3+Aq,   but  more   easily   by   dil. 
HNO3+Aq.    (Berzelius.) 

Cadmium  sulphomolybdate. 
Insol.  in  H2O.    (Berzelius.) 

Caesium    sulphomolybdate,    Cs2S,    3MoS4+ 

7H20. 

As  Rb  comp.    (Herschfinkel,  Dissert.  1907.) 
3Cs2S,  5MoS4.    (Herschfinkel.) 

Calcium  sulphomolybdate,  CaS,  3MoS3. 

Sol.  in  H2O.    (Berzelius.) 

CaMoS4.     More  sol.  in  H2O  than  CaS, 
3MoS3.   Known  only  in  solution.    (Berzelius.) 

Cerium  sulphomolybdate. 

Precipitate.    (Berzelius.) 

Cobalt  sulphomolybdate,  CoMoS4. 
Sol.  in  K2MoS4+Aq.    (Berzelius.) 

Cupric  sulphomolybdate. 
(Debray,  C.  R.  96.  1616.) 

Ferrous  sulphomolybdate,  FeMoS4. 
Sol.  in  H2O.    (Berzelius.) 

Ferric  sulphomolybdate,  Fe2(MoS4)3. 
Sol.  in  K2MoS4+Aq. 

Lead  sulphomolybdate. 
Ppt.    (Berzelius.) 


Lithium  sulphomolybdate. 

Not  deliquescent,  but  very  easily  sol.  in 
H2O.  (Berzelius.) 

Magnesium  sulphomolybdate,  MgMoS4. 
Sol.  in  K2MoS4+Aq.    (Berzelius.) 

Manganous  sulphomolybdate,  MnMoS4. 
Sol.  in  H2O.    (Berzelius.) 

Mercurous  sulphomolybdate,  Hg2MoS<  (?). 
Ppt. 

Mercuric  sulphomolybdate,  HgMoS4. 
Insol.  in  K2MoS4+Aq. 

Nickel  sulphomolybdate,  NiMoS4. 
Sol.  in  K2MoO4+Aq.    (Berzelius.) 

Potassium  sulphomolybdate,  basic,  K6Mo2S9. 
Easily  sol.  in  H2O.     Insol.  in  alcohol  and 
ether.    (Kruss,  B.  16.  2050.) 

Potassium  sulphomolybdate,  K2MoS4. 

Sol.  in  H2O,  from  which  it  is  precipitated 
by  alcohol.  (Berzelius.) 

Rubidium  sulphomolybdate,  3Rb2S,  8MoS3  + 
30H2O. 

Very  si.  sol.  in  H2O.  Sol.  by  addition  of 
NH3.  (Herschfinkel,  Dissert.  1907.) 

5Rb2S,  6MoS2.    (Herschfinkel.) 

Silver  sulphomolybdate,  Ag2MoS4. 
Ppt. 

Sodium  sulphomolybdate,  Na2MoS4. 

Sol.  in  H2O,  and  not  precipitated  by  al- 
cohol from  aqueous  solution.  (Berzelius.) 

Strontium  sulphomolybdates. 

Exactly  analogous  to  the  Ba  salts,  which 
see.  (Berzelius.) 

Zinc  sulphomolybdate. 

Ppt.    Insol.  in  H2O.    (Berzelius.) 

Mowosulphomolybdic  acid.] 

Sodium  rnonosulphomolybdate,  Na2MoO3S. 

Rather  hygroscopic.  Sol.  in  H2O;  forms 
deep  blue  solution  with  H2SO4.  Sol.  in 
HC2H3O2+Aq.  (Kruss,  A.  225.  1.) 

ZH'sulphomolybdic  acid. 

Ammonium  ^sulphomolybdate. 

(NH4)2Mo02S2. 

SI.  sol.  in  cold,  easily  in  hot  H2O.  Insol. 
in  sat.  NH4Cl+Aq  and  absolute  alcohol. 

Aqueous  solution  is  decomp.  by  boiling. 
(Bodenstab,  J.  pr.  78.  186.) 


SULPHONOSMATE,  POTASSIUM 


887 


Potassium  cfosulphomolybdate,  K2MoO2S2. 

Very  sol.  in  H2O  and  alcohol.  Sol.  in 
HC2H3O2+Aq.  (Kriiss,  B.  16.  2046.) 

Tn'sulphomolybdic  acid. 

Ammonium    hydrogen     Zn'sulphopyromolyb- 

date,  NH4HMo2O4S3. 
Precipitate.      Insol.    in    alcohol    or    CS2 
(Kriiss,  B.  16.  2047.) 

Potassium  hydrogen  Znsulphopyromolybdate 

KHMo204S3. 

Very  easily  sol.  in  H2O.  (Kriiss,  B.  16, 
2048.) 

Sodium    hydrogen     2nsulphdp?/romolybdate, 

NaHMo2O4S3. 
Precipitate.    Much  more  sol.  in  H2O  than 
the  NH4  compound.    (Kriiss,  B.  16.  2047.) 

Potassium  sulphoinolybdate,  K8Mo4S9O7. 

Sol.  in  H2O,  HC2H30%  and  H2SO4.  (Kruss 
B.  17.  1771.) 

Pewtasulphomolybdic  acid. 

Potassium  pentasulphomolybdate,  KMoS6. 

Sol.  in  warm  H2O.  (Hofmann,  Z.  anorg. 
1896,  12.  62.) 

Persulphomolybdic  acid,  H2MoS5. 

Precipitate.  Insol.  in  H2O,  alcohol,  ether, 
CS2,  and  acetic  acid. 

Decomp.  slowly  by  hot  H2SO4.  Sol.  in 
warm  KOH+Aq,  and  cold  K2S+Aq.  Not 
attacked  by  cold  KSH+Aq,  but  dissolves 
on  warming.  (Kriiss,  B.  17.  1773.) 

Ammonium  persulphomolybdate, 

(NH4)2MoS5. 

Very  si.  sol.  in  cold,  more  easily  in  hot 

JI2O.     Insol.  in  NH4OH+Aq.     (Berzelius.) 

Barium ,  BaMoS6. 

Insol.  in  boiling  H2O  or  dil.  HCl-fAq. 
(Berzelius.) 

Calcium . 

Difficultly  sol.  in  H2O.     (Berzelius.) 

Cerium . 

Precipitate.    (Berzelius.) 


Ferrous . 

Insol.  in  Fe  salts -fAq,  but  sol.  in  K2MoS6+ 
Aq.    (Berzelius.) 

Ferric . 

Ppt. 


Lithium  persulphomolybdate. 

SI.  sol.  in  cold,  easily  sol.  in  hot   H2O. 
(Berzelius.) 

Magnesium . 

Insol.  precipitate.     (Berzelius.) 

Nickel . 

Ppt.    Sol.  in  K2MoS6+Aq,  from  which  it 
separates  in  24  hours.    (Berzelius.) 

Potassium  — — ,  K2MoS6. 

Almost  insol.  in  cold,  more  sol.  in  hot  H2O. 
Insol.  in  cold  KOH+Aq.    (Berzelius.) 

Potassium  hydrogen ,  KHMoS6. 

Sol.  inH2O.    (Kruss.) 

Sodium ,  Na2MoS6. 

SI.  sol.  in  cold,  easily  in  hot  H2O.     (Ber- 
zelius.) 


Sodium  hydrogen 

(Kruss.) 


-,  NaHMoS5. 


Persulphomolybdic  acid,  HMoS6. 

Sol.  in  H2O.     (Hofmann,  Z.  anorg.  1896, 
12.  59.) 

Ammonium ,  NH4MoS6+H20. 

SI.  sol.  in  H2O  and  in  alcohol  with  decomp. 
(Hofmann.) 

Caesium  — — ,  CsMoS6 
Almost  insol.  in  H2O.     (Hofmann.) 

Potassium  — — ,  KMoS6. 
Sol.  in  H2O.    (Hofmann,) 

Thallium ,  TlMoS6. 

Insol.  in  H2O.    (Hofmann.) 

Sulphonosmic  acid. 

Potassium  sulphonosmate, 
7K20,  40s03,  10  S02. 

Sol.  in  H2O.    (Rosenheim,  Z.  anorg.  1899, 
21.  127.) 

+3H2O.    Sol.  in  H2O.    (Rosenheim.) 
+7H2O.    Easily  sol.  in  H2O;  decomp.  in 
aq.  solution  at  70  .    (Rosenheim.) 

11K2O,  4OsO3, 14SO2+7H2O.    Sol.  in  H2O. 
Rosenheim.) 

Sodium  sulphonosmate, 

3Na2O,  OsO8,  4SO2+5H2O. 
Easily  sol.  in  H2O;  decomp.  in  aq.  solution. 
Rosenheim.) 


888 


SULPHOPALLADIC  ACID 


Sulphopalladic  acid. 

Potassium  palladious  sulphopalladate,  K2S, 

Pd2S,  PdS2=K2Pd3S4. 
Insol.  in  H2O.    Moderately  cone.  HCl+Aq 
dissolves  out  K  without  evolution  of  H2S. 
(Schneider,  Pogg.  141.  526.) 

Silver  sulphopalladate,  Ag2PdS3. 
(Schneider.) 

Silver    palladious    sulphopalladate,    Ag2S, 

Pd2S,  PdS2=Ag2Pd3S4. 
Extraordinarily  stable.    (Schneider.) 

Sodium  sulphopalladate,  Na2PdS3. 

Slowly  sol.  in  H2O.     Insol.  hi  alcohol. 
(Schneider,  Pogg.  141.  520.) 

Sulphophosphide  of  M. 
See  M  phosphosulphide. 


Sulphophosphamic  acid,  1 
See  Thiophosphamic  acid. 

OH 
Sulphophosphodiamic  acid,  PS/j^jV  0 

See  Thiophosphocfo'amic  acid. 

SulphophosphoJn'amide,  PS(NH2)3. 
See  Thiophosphoryl  Znamide. 

Sulphophosphoric  acid,  H3PSO3. 
See  Thiophosphoric  acid. 
H3PS4.    Known  only  in  its  salts. 

Ammonium  sulphophosphate,  (NH4)3PS4. 

Stable  in  the  air.  (Ephraim,  B.  1911, 
44.  3408.) 

Antimony  sulphophosphate,  SbPS4. 

Insol.  in  H2O,  alcohol,  ether,  CS2,  HC1+ 
Aq,  dil.  H2SO4+Aq,  CeHe,  or  HC2H3O2. 
Decomp.  by  boiling  with  cone.  HNO3+Aq, 
H2S04,  aqua  regia,  KOH,  NaOH  or  NH4OH 
+Aq.  (Glatzel,  B.  24.  3886.) 

Arsenic  sulphophosphate,  AsPS4. 

Insol.  in  H2O,  alcohol.  HCl+Aq,  etc.  De- 
comp. by  warm  HNO3,  aqua  regia,  dil 
H2S04;  also  sol.  in  KOH  or  NH4OH+Aq 
(Glatzel,  Z.  anorg.  4.  186.) 

Barium  sulphophosphate,  Ba3(PS4)2+xH20. 
(Ephraim,  B.  1911,  44.  3409.) 

Bismuth  sulphophosphate,  BiPS4. 

Insol.  in  H2O,  alcohol,  ether,  CS2,  benzene 
HC2H3O2,  or  dil.  H2SO4+Aq.  Decomp.  by 
boiling  HCl+Aq,  cone.  H2SO4,  HNO3,  or 
aqua  regia;  also  by  NaOH,  KOH,  or  NH4OH 
+Aq.  (Glatzel,  Z.  anorg.  4. 186.) 


Cadmium  sulphophosphate,  Cd3(PS4)2. 

Insol.  in  H2O,  alcohol,  ether,  benzene, 
CS2,  and  HC2H3O2.  Decomp.  by  hot  HC1+ 
Aq.  Very  si.  attacked  by  dil.  H2SO4+Aq. 
Slowly  sol.  in  hot  HNO3,  rapidly  in  aqua  regia 
or  hot  cone.  H2SO4.  (Glatzel,  Z.  anorg.  4. 
186.) 

Cuprous  sulphophosphate,  Cu3PS4. 

Insol.  in  H2O,  alcohol,  etc.;  also  in  HC1  or 
dil.  H2SO4+Aq.  Decomp.  by  HNO3,  aqua 
regia,  etc.,  not  by  KOH  or  NaOH+Aq. 
'Glatzel.) 

Ferrous  sulphophosphate,  Fe3(PS4)2. 

Insol.  in  H2O,  alcohol,  ether,  etc.;  insol.  in 
BC1  or  hot  dil,  H2SO4+Aq.  Decomp.  by 
HNO3,  aqua  regia,  or  cone.  H2SO4.  Not 
attacked  by  KOH  or  NH4OH+Aq.  (Glat- 
zel.) 

Lead  sulphophosphate,  Pb3(PS4)2. 

Insol.  in  H2O,  alcohol,  etc.  Decomp.  by 
warm  HCl+Aq,  cone.  HNO3+Aq;  not  at- 
tacked by  NH4OH+Aq;  si.  decomp.  by  KOH 

+Aq.    (Glatzel.) 

Manganous   sulphophosphate,    Mn3(PS4)2. 

Insol.  in  H2O,  alcohol,  ether,  benzene,  CS2, 
or  HC2H3O2.  Not  attacked  by  HCl+Aq. 
Sol.  in  HNO3  or  aqua  regia,  with  separation 
of  S.  Not  attacked  by  dil.  H2SO4+Aq. 
(Glatzel,  Z.  anorg.  4.  186.) 

Mercuric  sulphophosphate,  Hg3(PS4)2. 

Insol.  in  H2O,  alcohol,  etc.;  also  in  HC1, 
dil.  HNO3,  or  H2SO4+Aq.  Not  attacked  by 
cone.  HNO3  or  aqua  regia;  easily  sol.  in 
HNO3+Br2+Aq.  (Glatzel.) 

Nickel  sulphophosphate,  Ni3(PS4)2. 
As  the  ferrous  salt.     (Glatzel.) 

Potassium  sulphophosphate,  K3PS4+H2O. 

Easily  sol.  in  H2O.  (Ephraim,  B.  1911,  44. 
3407.) 

Silver  sulphophosphate,  Ag3PS4. 

Insol.  in  H2O,  alcohol,  etc.;  also  in  HC1, 
HNO3,  or  dil.  H2SO4+Aq.  Decomp.  by 
cone.  H2SO4,  and  aqua  regia.  (Glatzel.) 

Sodium  sulphophosphate,  Na3PS4+8H2O. 

Decomp.  by  H2O. 

Sol.  in  Na2S+Aq.  (Glatzel,  Z.  anorg. 
1905,  44.  65.) 

Thallous  sulphophosphate,  T13PS4. 

Insol.  in  H2O,  alcohol,  etc.  Sol.  in  HC1, 
dil.  H2SO4+Aq,  etc.  Not  attacked  by 
NH4OH+Aq;  si.  decomp.  by  cone.  KOH+ 
Aq.  (Glatzel.) 


SULPHOPHOSPHITE,  SILVER 


Tin  (stannous)  sulphophosphate,  Sn3(PS4)2. 
Insol.  in  H2O,  alcohol,  etc.  Insol.  in  dil. 
H2SO4  or  HCl+Aq.  Decomp.  by  HNO3+ 
Aq,  aqua  regia,  NH4OH,  or  KOH+Aq. 
(Glatzel.) 

Zinc  sulphophosphate,  Zn3(PS4)2. 

Insol.  in  H2O,  alcohol,  ether,  etc.  Sol.  in 
HCl+Aq  or  dil.  H2SO4+Aq.  Easily  at- 
tacked by  KOH+Aq;  si.  decomp.  by  NH4OH 
+Aq.  (Glatzel.) 

Sulphop?/rophosphoric  acid. 

Aluminum  sulphop?/rophosphate,  A12P2S7. 

Decomp.  in  moist  air. 

Violently  decomp.  by  H2O  or  acids.  (Fer- 
rand,  A.  ch.  1899,  (7)  429.) 

Cadmium  ,  Cd2P2S7. 

Decomp.  in  moist  air. 

Not  attacked  by  cold  acids.    (Ferrand.) 

Chromium  — — •,  Cr2P2S7. 
Decomp.  in  moist  air. 
Not  readily  attacked  by  acids.  (Ferrand.) 

Cuprous ,  Cu4P2S7. 

Not  attacked  by  cold  H2SO4  or  boiling 

HC1.     (Ferrand.) 

Sol.  in  hot  cone.  HNO3.    (Ferrand.) 

Sol.  in  alkalies,  and  in  all  acids  except  HC1. 

(Ferrand,  C.  R.  1896,  122.  886.) 

Ferrous  ,  Fe2P2S7. 

Insol.  in  cold  acids. 

SI.  attacked  by  boiling  HC1  or  hot  KOH  + 

Decomp.  by  fused  KOH.  (Ferrand,  A. 
ch.  1899,  (7)  17.  410.) 

Lead ,   Pb2P2S7. 

Not  attacked  by  cold  HNO3.     (Ferrand,) 

Mercurous  — • — •,  Hg4P2S7. 

Decomp.  by  moist  air  or  hot  HNO3.  (Fer- 
rand.) 

Almost  insol.  in  acids;  decomp.  by  H2O 
and  moist  air.  (Ferrand,  C.  R.  1896,  122. 
888.) 

Nickel ,  Ni2P2S7. 

Decomp.  by  H2O  and  by  cone.  HNO3  at 
150°  in  a  sealed  tube.  (Ferrand,  A.  ch. 
1899,  (7)  17.  418.) 

Silver ,  Ag4P2S7. 

Not  decomp.  by  H2O. 

Decomp.  by  aqua  regia. 

Not  attacked  by  HNO3.     (Ferrand.) 

Zinc ,  Zn2P2S7. 

Decomp.  in  moist  air. 
Decomp.  by  H2O. 


Violently  attacked  by  cold  HNO3.  (Fer- 
rand.) 

Sulphophosphorous  acid, 

H3PSO2=SPOH(?). 

OH 

See  Thiophosphorous  acid. 
H3PS3.    Known  only  in  its  salts. 

Aluminum  sulphophosphite,  A13(PS3)2. 

Very  unstable. 

Decomp.  in  the  air.  (Ferrand,  C.  R.  1896, 
122.  622.) 

Barium   sulphophosphite,    Ba3(PS3)2+zH2O. 

Sol.  in  dil.  acids. 

Insol.  in  alcohol.  (Ephraim,  B.  1911,  44. 
3412.) 

Chromous  sulphophosphite,  Cr3(PS3)2. 

Easily  attacked  by  hot  cone.  HNO3  or 
aqua  regia. 

Decomp.  by  boiling  NaOH+Aq.  (Fer- 
rand, A.  ch.  1899,  (7)  17.  419.) 

Quite  stable  in  moist  air;  very  slowly  at- 
tacked by  acids.  (Ferrand,  C.  R.  1896,  122. 
622.) 

Cuprous  sulphophosphite,  Cu3PS3. 

Not  attacked  by  H2O  or  hot  cone.  HC1. 

SI.  attacked  by  cold  fuming  HNO3. 

Violently  attacked  by  HNO3,  aqua  regia 
and  boiling  cone.  H2SO4. 

Not  attacked  by  boiling  NaOH+Aq. 
(Ferrand,  A.  ch.  1899,  (7)  17.  398.) 

Fairly  stable;  decomp.  by  damp  air.  (Fer- 
rand, C.  R.  1896,  122.  621.) 

Iron  (ferrous)  sulphophosphite,  Fe3(PS3)2. 

Very  stable  and  resists  the  action  of  alkalies 
and  acids.  (Ferrand,  C.  R.  1896,  122.  622.) 

Insol.  in  cold  acids  or  hot  NCI. 

Sol.  in  hot  fuming  HNO3. 

Insol.  in  hot  40%  KOH+Aq.  (Ferrand, 
A.  ch.  1899,  (7)  17.  412.) 

Mercuric  sulphophosphite,  Hg3(PS3)2. 

Decomp.  in  moist  air. 

Not  attacked  by  cold  HNO3.  Decomp. 
byhotHNO3.  (Ferrand.) 

Unstable  in  the  air. 

Very  slowly  attacked  by  acids.  (Ferrand, 
C.  R.  1896,  122.  622.) 

Nickel  sulphophosphite,  Ni3(PS3)2. 
Unstable  in  the  air. 
Attacked  slowly  by  HNO3.    (Ferrand.) 

Silver  sulphophospbite,  Ag3PS3. 

Insol.  in  most  reagents.  (Ferrand.  C.  R. 
1896,  122.  622.) 

Not  decomp.  by  H2O. 

Not  easily  attacked  by  acids.  (Ferrand, 
A.  ch.  1899,  (7)  17.  414.) 


890 


SULPHOPHOSPHITE,  SODIUM 


Sodium  sulphophosphite,  Na3PS3+zH2O. 

Very  sol.  in  H2O,  probably  with  decomp. 
(Ephraim,  B.  1911,  44.  3410.) 

Zinc  sulphophosphite,  Zn3(PS3)2. 

Decomp.  in  moist  air. 

SI.  attacked  by  H2O. 

Decomp.  by  HNO3.  (Ferrand,  A.  ch. 
1899,  (7)  17.  422.) 

Very  unstable  in  the  air,  and  attacked 
violently  by  acids.  (Ferrand,  C.  R.  1896, 
122.622.)  ' 

Sulphoplatinic  acid,  H2Pt4S6. 

Insol.  in  H2O,  but  decomp.  on  air. 
(Schneider,  Pogg.  138.  604.) 

H4Pt3S6.  Insol.  in  H2O,  but  decomp. 
very  rapidly  on  air.  (Schneider.) 

Copper  sulphoplatinate,  2CuS,  2PtS,  PtS2. 

Insol.  in  H2O.  HC1,  HNO3,  or  aqua  regia 
dissolve  out  part  of  the  Cu.  (Schneider, 
Pogg.  139.  661.) 

Lead  sulphoplatinate,  2PbS,  2PtS,  PtS2. 

Insol.  in  hot  or  cold  H2O  or  HCl+Aq. 
HNO3+Aq  dissolves  out  Pb  partly;  aqua 
regia  dissolves  completely  with  difficulty. 
(Schneider,  Pogg.  139.  662.) 

Mercuric    sulphoplatinate    chloride,    2HgS, 

2PtS,  PtS2,  2HgCl2. 

Insol.  in  H2O;  not  attacked  by  HCl+Aq, 
and  only  partially  sol.  in  boiling  aqua  regia. 
(Schneider.) 

Potassium  sulphoplatinate,  K2Pt4S6. 

Insol.  in  H2O.  HCl+Aq  dissolves  out  K 
without  evolution  of  H2S. 

Composition  its  potassium  platinous  sul- 
phoplatinate, K2S,  3PtS,  PtS2.  (Schneider, 
Pogg.  138.  604.) 


Silver  sulphoplatinate,  2Ag2S,  2PtS,  PtS2. 
Insol.  in  H20  or  HCl+Aq.  HNO3+Aq 
dissolves  out  Ag  on  warming.  Aqua  regia 
decomp.  with  formation  of  AgCl.  (Schnei- 
der, Pogg.  138.  664.) 

Sodium  sulphoplatinate,  Na4Pt3S6  =  2Na2S, 
2PtS,  PtS2. 

Decomp.  by  hot  H2O,  with  residue  of 
PtS2.  (Schneider.) 

Na2Pt3S6  =  Na2S,  PtS,  2PtS2.  Insol.  in 
H2O.  (Schneider,  J.  pr.  (2)  48.  418.) 

Thallium  sulphoplatinate,  2T12S,  2PtS,  PtS2. 
Insol.  in  cold  H2O.    Dil.  acids  dissolve  out 
all   the   thallium.      (Schneider,    Pogg.    138. 
626.) 


Sulphoplatinous  acid,  H2PtS2. 

Known  only  in  solution  in  H2O,  which 
soon  decomposes.  (Schneider,  J.  pr.  (2) 
48.  424.) 

Sodium  sulphoplatinite,  Na2PtS2. 

Sol.  in  H2O  with  decomp.  (Schneider,  J. 
pr.  (2)  48.  420.) 

H4Na2(PtS2)3.  Sol.  in  H2O,  from  which  it 
is  pptd.  by  alcohol.  (Schneider.) 

Sulphoselenantimonous  acid. 
See  Selenosulphantimonous  acid. 

Sulphoselenarsenic  acid. 
See  Selenosulpharsenic  acid. 

Sulphoselenostannic  acid. 
See  Selenosulphostannic  acid. 

Sulphoselenoxyarsenic  acid. 
See  Selenosulphoxyarsenic  acid. 

Sulphoselenyl  chloride,  SSeO3Cl4. 

Deliquescent;  decomposed  by  H2O.  (Claus- 
nitzer,  B.  11.  2007.) 

Afetasulphosilicic  acid. 

Sodium  metosulphosilicate,  Na2SiS3. 

Decomp.  by  H2O.  (Hempel,  Z.  anorg. 
1900,  23.  41.) 

Sulphostannic  acid,  H2SnS3. 

Ppt.     (Kiihn,  A.  84.  110.) 

Does  not  exist.  (Storch,  W.  A.  B.  98. 
2b.  236.) 

Ammonium    sulphostannate,     (NH4)2S, 
3SnS2+6H2O. 

Easily  sol.  in  H2O,  and  easily  decomp. 
(Ditte,  C.  R.  96.  641.) 

(NH4)2SnS3+3H2O,  and  +7H2O.  De- 
comp. by  acid.  (Stanek,  Z.  anorg.  1898,  17. 
124.) 

Barium  sulphostannate,  BaSnS3+8H2O. 
Sol.  in  cold  H2O.    (Ditte,  C.  R.  96.  641.) 

Calcium  sulphostannate,  2CaS,  SnS2+14H2O. 
Sol.  in  H2O.    (Ditte,  C.  R.  96.  641.) 


s  sulphostannate,  4PtS,  SnS2. 
Not  decomp.  by  acids.    (Schneider,  J.  pr. 
(2)  7.  214.) 

Platinum   potassium   sulphostannate,   3PtS, 

K2S,  SnS2. 

Insol.  in  cold  H2O.  Dil.  HC1  or  HC2H3O2 
+Aq  dissolves  out  all  the  potassium.  (Sch- 
neider, Pogg.  136.  109.) 


SULPHOSTANNATE,  PLATINUM  SODIUM 


891 


Platinum     sodium     sulphostannate,     3PtS, 

Na2S,  SnS2. 

Insol.  in  cold  H2O.  (Schneider,  Pogg.  136. 
109.) 

Potassium  sulphostannate,  K2SnS3. 
Sol.  in  H2O.    (Kuhn,  A.  84.  110.) 
+3H2O.     (Ditte,  C.  R.  96.  641.) 
K4SnS4+4H2O.     Sol.   in  H2O:   pptd.   by 

alcohol.    (Weinland,  Z.  anorg.  1898,  17.  419.) 

Sodium  sulphostannate,  Na2SnS3+2H2O. 
SI.  sol.  in  H2O.    (Kuhn,  A.  84.  110.) 
+3H2O.    (Ditte,  C.  R.  95.  641.) 
+7H2O.     Sol.  in  H2O.     (Horing,  Zeitsch. 

Pharm.  1851.  120.) 

Na4SnS4 + 12H2O.    Melts  in  crystal  H2O  on 

heating.    Very  sol.  in  H2O.    (Kuhn.) 

Strontium  sulphostannate,  SrSnS3  +  12H2O. 
Sol.  in  H2O.     (Ditte,  C.  R.  95.  641.) 

Thallium  sulphostannate,  Tl4SnS4. 

Ppt.  Practically  insol.  in  H2O.  (Hawley, 
J.  Am.  Chem.  Soc.  1907,  29.  1011.) 

ZH'sulphopersulphuric  acid. 

Sodium  efosulphopersulphate,  Na2S4O8. 

Sol.  in  H2O.  Cryst.  in  cold  with  2H2O. 
(Villiers,  C.  R.  106.  851,  1354.) 

Contains  4H  more  and  is  sodium  tetra- 
thionate,  NaS4O6,  2H2O.  (Villiers,  C.  R. 
108.  402.) 

Sulphotelluric  acid; 

Mercurous  sulphotellurate,  3Hg2S,  TeS2. 
Ppt. 

Mercuric ,  3HgS,  TeS2. 

Ppt.     (Berzelius.) 

Potassium ,  K2TeS4. 

Sol.  in  H2O.     (Oppenheim,  J.  pr.  71.  279.) 

Sodium . 

Sol.  in  H2O.     (Oppenheim.) 

Sulphotellurous  acid. 

Ammonium  sulphotellurite,  3(NH4)2S,  TeS2. 
Decomp.  on  air.    Sol.  in  H2O. 

Barium . 

Very  slowly  sol.  in  H2O. 

Calcium . 

Somewhat  sol.  in  H2O. 

Cerium . 

Insol.  ppt. 


Cobalt  sulphotellurite,  Co3TeS6. 
Ppt. 

Copper ,  Cu3TeS6. 

Ppt. 

Ferrous . 

Ppt. 

Ferric . 

Ppt. 

Lead . 

Ppt. 

Lithium . 

Sol.  in  H2O. 

Magnesium •. 

Sol.  in  H2Q  and  alcohol. 

Manganous •. 

Ppt. 

Potassium ,  3K2S,  TeS2. 

Sol.  in  H2O. 

Silver ,  3Ag2S,  TeS2. 

(Berzelius.) 

Sodium . 

Sol.  in  H2O. 

Strontium . 

Sol.  in  H2O. 

Zinc •,  3ZnS,  TeS2. 

Ppt.     (Berzelius.) 

Sulphotungstic  acid. 

Ammonium  sulphotungstate,  (NH4)2WS4. 

Very  deliquescent.  Easily  sol.  in  H2O,  and 
still  more  easily  in  NH4OH+Aq.  (Corleis. 
A.  232.  244.)  *»|) 

More  sol.  in  pure  H20  than  in  H2O  acidified 
with  HC1.  Decomp.  slowly  on  air.  |(Ber- 
zelius.) 

Barium . 

Sol.  in  BaS+Aq. 

Cadmium ,  CdWS4. 

Ppt.    (Berzelius.) 

Calcium •. 

Sol.  in  H2O  and  alcohol.    (Berzelius.) 

Cobalt ,  CoWS4. 

SI.  sol.  in  H2O. 


892 


SULPHOTUNGSTATE,  COPPER 


Copper  sulphotungstate,  CuWS4. 
Ppt. 

Glucinum ,  G1WS4. 

Sol.  in  H2O(?). 

Ferrous  — ,  FeWS4. 
Sol.  in  H2O. 

Ferric . 

Ppt. 

Lead ,  PbWS4. 

Ppt.     (Berzelius.) 

Magnesium •,  MgWS4. 

Easily  sol.  in  H2O  or  alcohol. 

Manganous •,  MnWS4. 

Sol.  in  H2O.    (Berzelius.) 

Mercurous  — — . 
Ppt.    (Berzelius.) 

Mercuric -,  HgWS4. 

Ppt.     (Berzelius.) 

Nickel  — ,  NiWS4. 
Ppt.    (Berzelius.) 

Potassium ,  K2WS4. 

Sol.  in  H2O.  Alcohol  precipitates  from 
aqueous  solutions,  but  is  not  entirely  insol. 
in  alcohol.  (Berzelius.) 

Very  sol.  in  H2O.     (Corleis,  A.  232.  264.) 

Potassium  —  nitrate,  K2WS4,  KN03. 

Very  sol.  in  cold  or  hot  H2O,  from  which 
it  is  precipitated  by  alcohol.  (Berzelius.) 

Potassium    tungstate,    K2W02S2  = 

K2WS4,  K2W04. 

Easily  sol.  in  H2O.  Not  precipitated  by 
alcohol.  (Berzelius.) 

Is  potassium  ^nsulphotungstate,  K2WOS3, 
which  see.  (Corleis,  A.  232.  244.) 

Silver ,  Ag2WS4. 

Ppt.     (Berzelius.) 

Sodium  — ,  Na2WS4. 

Very  sol.  in  H2O;  less  sol.  in  alcohol.  (Ber- 
zelius.) 

Very  deliquescent.     (Corleis,  A.  232.  264.) 

Strontium . 

Sol.  in  H2O,  and  in  SrS+Aq. 

Stannous ,  SnWS4. 

Ppt.     (Berzelius.) 

Stannic ,  SnWS6. 

Ppt.     (Berzelius.) 


Zinc  sulphotungstate,  ZnWS4. 

Sol.  in  H2O  with  subsequent  pptn.  (Ber- 
zelius.) 

Afonosulphotungstic  acid. 

Potassium  raonosulphotungstate, 

K2WOS+H2O. 

Deliquescent  in  moist  air.  Very  sol.  hi 
H20.  (Corleis,  A.  232.  244.) 

ZH'sulphotungstic  acid. 

Ammonium  ^sulphotungstate,  (NH4)2WO2S2. 
Sol.  in  H2O  and  alcohol.     (Berzelius.) 
Decomp.  easily  when  moist.     (Corleis,  A. 

232.  264.) 

Tn'sulphotungstic  acid. 

Potassium     tfn'sulphotungstate,     K2WOS3-f- 

H2O. 

Hygroscopic.  Effloresces  on  dry  air  and 
easily  decomposed.  Easily  sol.  in  H2O.  (Cor- 
leis, A.  232.  244.) 

Sulphovanadic  acid,  V2O5,  3SO3+3H2O. 

See  Vanadiosulphuric  acid,  and  Sulphate, 
vanadium. 

Sulphovanadates. 

Alkali  sulphovanadates  are  sol.  in  H2O. 
Ca,  Sr,  and  Ba  sulphovanadates  are  si.  sol.  in 
H2O,  and  all  other  sulphovanadates  are  insol. 
inH2O.  (Berzelius.) 

Ammonium  sulphovanadate,  (NH4)3VS4. 

Easily  sol.  in  H2O.  Very  si.  sol.  in  cone. 
NH4SH  +Aq.  Insol.  in  ether,  CS2,  or  CHC13. 
(Kriiss  and  Ohnmais,  A.  263.  46.) 

See  also  Sulphoxyvanadic  acid. 

Sodium  pentasulphopyrovanadate,  Na4V2O2S5. 
Hydroscopic;  sol.  in  H2O  with  rapid  de- 
comp.    (Locke,  Am.  Ch.  J.  1898,  20.  375.) 

Sulphoxyantimonic  acid. 

Potassium  sulphoxyantimonate,  K2HSbO2S2 

+2H20. 

Sol.  in  hot,  less  sol.  in  cold  H2O.  Decomp. 
by  cold  H2O.  (Weinland  and  Gutmann,  Z. 
anorg.  1898,  17.  414.) 

Sulphoxyarsenic  acid,  H3AsO3S. 

Known  only  in  aqueous  solution.  (McCay, 
Am.  Ch.  J.  10.  459.) 

Ammonium   monosulphoxyarsenate, 

(NH4)3AsSO3+3H2O. 

Decomp.  in  the  air;  sol.  in  H2O,  decomp.  on 
boiling.  (Weinland,  B.  1896,  29.  1009.) 


SULPHOXYARSENATE,  SODIUM  STRONTIUM 


893 


Very  sol.  in  H2O;  insol.  in  alcohol;  decomp. 
in  aq.  solution  and  also  in  the  air.  (Weinland, 
Z.  anorg.  1897,  14.  53.) 

Decomp.  in  the  air.  (McLauchlan,  B. 
1901,  34.  2166.) 

Ammonium  hydrogen  monosulphoxyarsenate, 

(NH4)2HAsSO3. 
Ppt.    (McLauchlan,  B.  1901,  34.  2168.) 

Barium  monosulphoxyarsenate.  BaHAs03  + 
10H20. 

(Preis,  A.  257.  184.) 

Ba3(AsSO3)2+6H2O.  Ppt.  (Weinland,  Z. 
anorg.  1897,  14.  54.) 

Barium  efo'sulphoxyarsenate,  Ba3(AsS2O2)2  + 
4H2O. 

Ppt.    (Preis,  A.  257.  185.) 
+6H2O.    (Weinland  and  Rumpf,  Z.  anorg. 
1897,  14.  64.) 

Barium  potassium  ^n'sulphoxyarsenate, 

KBaAsS3O+7H2O. 
Ppt.    (McCay,  Z.  anorg.  1904,  41.  469.) 

Barium  sodium  monosulphoxyarsenate, 

BaNaAsSO3+9H2O. 
Ppt.    (Weinland,  Z.  anorg.  1897,  14.  55.) 

Barium  sodium  sulphoxyarsenate, 

Ba7Na2As5O7S14 
(McCay  and  Foster,  Z.  anorg.  1904,  41.  467.) 

Calcium  ^n'sulphoxyarsenate,  Ca3(AsS3O)2  + 
20H2O. 

Ppt.  (McCay  and  Foster,  Z.  anorg.  1904, 
41.  463.) 

Potassium  monosulphoxyarsenate,  K3AsSO3. 

Hydroscopic.  (Weinland,  B.  1896,  29. 
109.) 

Sol.  in  cone.  KOH+Aq,  free  from  carbon- 
ate; very  hydroscopic.  (Weinland,  Z.  anorg. 
1897,  14.  51.) 

Potassium  hydrogen  monosulphoxyarsenate. 
K2HAsSO3+2^H2O. 

Very  hygroscopic.  (Weinland  and  Rumpf, 
Z.  anorg.  1897,  14.  59.) 

KH2AsSO3.  Sol.  in  H2O;  solution  slowly 
decomp.  on  standing.  (McCay,  Am.  Ch.  j. 
10.  459.) 

Formula  given  by  Bouquet  and  Cloez  (A. 
ch.  (3)  13.  44)  is  K2H4As2S3O5. 

Potassium  disulphoxyarsenate,   K3AsS2O2  + 

10H20. 

Very  hydroscopic;  decomp.  by  H2O. 
(Weinland,  Z.  anorg.  1897,  14.  63.) 

Potassium   ^n'sulphoxyarsenate.   K3AsS3O  + 

7H20. 

Yellow  oil  which  cryst.  at  —20°.  (McCay 
and  Foster,  Z.  anorg.  1904,  41.  468.) 


Sodium  monosulphoxyarsenate,  Na3AsS03  + 
12H20. 

Easily  sol.  in  H2O.  (Preis,  A.  257.  180.) 
(McLaughl,an,  B.  1901,  34.  2170.) 

Sol.  in  H2O.    (Weinland,  B.  1896,  29.  1009.) 

SI.  efflorescent.  Insol.  in  alcohol.  (McCay, 
Z.  anorg.  1902,  29.  42.) 

Sol.  in  NaOH+Aq;  decomp.  by  boiling 
with  cone.  NaOH.  (Weinland,  Z.  anorg. 
1897,  14.  49.) 

Sodium  hydrogen  monosulphoxyarsenate, 
NaH2AsSO3. 

Deaomp.  by  H20;  insol.  in  alcohol.  (Wein- 
land, Z.  anorg.  1897,  14.  58.) 

Na2HAsSO3+8H2O.  Easily  sol.  in  H2O. 
(Preis.) 

Sodium  (^'sulphoxyarsenate,  Na3AsS2O2  + 
10H2O. 

Easily  sol.  in  H2O.    (Preis.) 

Sol.  in  H2O;  pptd.  by  alcohol.  (McCay,  B. 
1899,  32.  2472.) 

Not  decomp.  by  boiling  NaOH+Aq. 
(Weinland,  Z.  anorg.  1897,  14.  62.) 

Insol.  in  alcohol.  (McCay,  Z.  anorg.  1900. 
25.  461.) 

+11H2O.  (McLaughlan;  B.  1901,  34. 
2170.) 

Insol.  in  alcohol.  (McCay,  Z.  anorg.  1902, 
29.  46.) 

Sodium     frisulphoxyarsenate,     Na3AsS3O  + 

11H2O. 

Decomp.  by  H2O.  (McCay  and  Foster, 
Z.  anorg.  1904,  41.  454.) 

Sodium      ^nsulphoxydiarsenate,       As2O2S3, 

3Na2O+24H2O. 

Easily  sol.  in  H2O.    (Geuther,  A.  240.  208.) 
2As2O2S3,    Na2O+7H2O.      Sol.    in    H2O. 

(Nilson,  J.  pr.  (2)  14.  14.) 
Correct    composition    is    Na8Asi8S24O7+ 

30H2O.    (Preis.) 

Sodium    sulphoxyarsenate,    Na8Asi8S24O7  + 


30H2O=4Na2O,       6As2S2, 
30H2O. 

Decomp.  by  H2O.    Sol.  in  NH4OH  or  KOH 
+Aq,    (Preis,  A.  257.  187.) 

=  Sodium  oxyin'sulpharsenate  of  Nilson. 

Sodium  perc/asulphoxytefrarsenate, 

Nai2As4S5On  +48H2O. 
Less   sol.   in   H2O   than   other   sulphoxy- 
arsenates.    (Preis.) 

Sodium   strontium  in'sulphoxyarsenate. 
NaSrAsS3O  +  10H2O. 

Unstable.     (McCay  and  Foster.  Z.  anorg. 
1904,  41.  462.) 


894 


SULPHOXYAZOTIC  ACID 


Tn'sulphoxyazotic  acid,  ON(SO3H)3. 

Known  only  in  its  salts.  (Glaus,  A.,  158. 
52  and  194.) 

Has  the  formula  (SO3H)3N<Q>N(SO3H)3. 
(Raschig,  A.  241.  161.) 
Potassium  ^n'sulphoxyazotate,  ON(SO3K)3  + 
H20  =  (S03K)3N<°>N(S03K)3. 

Easily  sol.  in  H2O  without  decomp.,  even 
on  boiling.  (Claus,  A.  167.  210.) 

Sulphoxyphosphorous  acid, 

H 
H3PS2O  =  OPSH(?). 

SH 
See  Thiophosphorous  acid. 

Sulphoxyvanadic  acid. 

Ammonium  p^/roAezasulphoxyvanadate. 

(NH4)4V2S60. 

Sol.  in  H2O.  (Kriiss  and  Ohnmais,  A.  263. 
53.) 

Potassium  w/ro/iezasulphoxyvanadate. 
K4V2S60+3H20. 

Melts  in  crystal  H2O.  (Kriiss  and  Ohn- 
mais.) 

K8V4Si2O2+3H2O.  More  sol.  in  H2O  than 
preceding  comp;  (K.  and  O.) 

Sodium   or^otfnsulphoxyvanadate.    Na3VS3O 

+5H2O. 

Ve,ry  d,eliquesce,nt,  and  easily  sol.  in  H2O 
Somewhat  sol.  in  alcohol.  (Kriiss  and  Ohn- 
mais.) 

Sodium  or^omonosulphoxyvanadate, 

Na3VS93+10H2O. 

Less  sol.  in  H2O  than  other  sulphoxyvana- 
dates.  (K.  and  O.) 

Sulphur,  S. 

The  various  modifications  of  sulphur  have 
been  classified  in  many  different  ways,  and 
there  is  a  difference  of  opinion  as  to  whether 
certain  forms  are  true  allotropic  modifications 
or  not. 

The  data,  as  far  as  concerns  the  solubility, 
may  be  arranged  as  follows: — 

A.  Sol.  in  CS2.  1.  Rhombic,  octahedral,  or 
alpha  sulphur,  ordinary  sulphur.  Easily 
sol.  in  CS2,  etc.  See  below  for  solubility  in 
various  solvents. 

2.  Prismatic,  monoclinic,  or  beta  sulphur. 
Sol.  in  CS2,  but  is  converted  into  A.  1.  Pris- 
matic sulpnur  obtained  by  melting  brimstone 
is  not  wholly  sol.  in  CS2  on  account  of  admix- 
ture of  gamma  sulphur. 

Monoclinic  modification  is  more  sol.  than 
rhombic  in  CHC13,  ether  and  benzene.  (Meyer 
C.  C.  1903,  II.  481.) . 


3.  Soft  sulphur,  milk  of  sulphur. 

4.  Amorphous  sol.  sulphur  is  also  a  sepa- 
rate modification,   according  to   Berthollet. 

B.  Soft    sulphur,    obtained    by    strongly 
heating  and  quickly  cooling,  is  sol.  in  CS2, 
but  becomes  insol.  therein  by  repeatedly  dis- 
solving and  evaporating.     More  easily  sol. 
in  CS2  than  A,  1. 

C.  Insol.  in  CS2.     1.    By  action  of  strong 
light  on  S  in  CS2. 

2.  By  heating  to  b.-pt.,  cooling  suddenly, 
and  allowing  to  stand  until  hard.    Has  been 
called  gamma  sulphur,  but  is  a  mixture  of 
2/3  A,  4  and  Vs  insol.  S. 

3.  Insol.  S  in  flowers  of  sujphulr.     Con- 
verted into  A.   1  by  standing  3  days  with 
alcohol. 

According  to  Berthelot  (A.  ch.  (3)  49.  430) 
there  are  only  two  varieties  of  S.'  I.  "Octa- 
hedral," II.  "Amorphous." 

I.  Octahedral.    Sol.  in  CS2.    Scarcely  acted 
upon  by  KHSO3+Aq.    Converted  by  oxidis- 
ing agents  into  II. 

II.  Amorphous.    Insol.  in  neutral  solvents, 
viz.  H20,  alcohol,  ether,  CS2,  etc. 

Sol.  with  tolerable  rapidity  in  KHSO3+Aq. 
By  long  action  of  Na2S+Aq,  a  portion  is 
dissolved,  and  the  remainder  converted  into 
I.  Less  easily  oxidised  by  HNO3+Aq  than 
I.  Some  varieties  of  this  modification  are 
sol.  to  a  certain  extent  in  alcohol  and  ether, 
and  by  boiling  the  rest  of  the  sulphur  is  con- 
verted into  I;  also  by  long-continued  con- 
tact with  cold  alcohol.  Berthelot  holds  that 
the  modification  is  changed  before  dissolving. 
Solutions  of  the  alkalies,  alkali  salts,  and 
alkali  sulphides  change  insol.  into  sol.  sulphur. 
(Berthelot.) 

Elastic  sulphur  obtained  by  pouring  mol- 
ten sulphur  at  a  temp,  of  over  260°  into  H2O 
contains  35%,  or  more  of  a  modification  of  S 
which  is  insol.  in  CS2,  hot  or  cold,  but  sol. 
in  absolute  alcohol;  this  modification  can 
be  converted  back  into  ord.  sulphur  by  heat- 
ing to  100°.  (Pelouze  and  Fremy.)  (See 
C.  2.) 

This  modification  can  be  obtained  also 
by  action  of  HC1  on  thiosulphates.  (Fordos 
and  Ge"lis.) 

The  soft  pasty  sulphur  obtained  by  decom- 
position of  H2S  by  SO2  forms  an  almost 
clear  emulsion  (pesudo-solution)  with  H2O, 
from  which  it  is  pptd.  by  various  salts  and 
substances  which  have  no  chemical  affinity 
for  it.  23  pts.  S  combine  in  this  way  with 
100  pts.  H2O.  When  pptd.  by  saline  S9lu- 
tions,  some  of  the  S  remains  in  solution. 
When  solution  is  exposed  to  the  light,  S 
gradually  separates  out;  also  on  boiling  the 
same  takes  place.  The  above  pseudo-solu- 
tion is  pptd.  by  mineral  acids,  and  the  pptd. 
S  may  still  be  dissolved  in  fresh  water,  if  not 
left  in  contact  for  some  time  with  the  acid. 
Also  pptd.  by  K  salts,  with  loss  of  power 
of  forming  pseudo-solutions.  Pptd.  by  NH4 
and  Na  salts  without  losing  that  power. 


SULPHUR 


895 


Alkali  hydrates,  carbonates,  or  sulphides 
convert  it  into  insol.  S. 

The  solution  may  be  mixed  with  alcohol 
without  change.  Decomp.  by  long  shaking 
with  napthha  or  oil  of  turpentine.  The 
pseudo-solution  combines  with  CS2,  forming 
an  emulsion  which  subsequently  decomposes. 
The  S  itself  is  only  partially  sol.  in  CS2. 
(Selmi,  J.  pr.  57.  49.) 

By  treatment  of  amorphous  "insoluble"  S 
with  CS2  or  CC14,  a  small  part  goes  into  solu- 
tion, the  amount  being  dependent  on  the  time 
of  contact  with  the  temp.,  and  nature  of  the 
solvent,  but  independent  of  the  amount  of 
the  solvent.  It  is  assumed  that  this  is  due 
to  a  partial  change  of  the  "insoluble"  into 
soluble  S.  (Wigand,  Z.  phys.  Ch.  1910,  75. 
235.) 

"Delta"  sulphur.  Partly  sol.  in  H2O. 
(Debus,  Chem.  Soc.  63.  18.) 

A  colloidal  form  wholly  sol.  in  H2O  exists, 
which,  however,  decomposes  very  easily. 
(Engel,  C.  R.  112.  866.) 

Black  sulphur.  Insol.  in  alcohol,  ether,  CS2, 
fatty  oils  even  at  200°,  cold  alkali  hydroxides 
+Aq,  H2SO4,  HN03,  or  aqua  regia.  (Knapp, 
J.  pr.  (2)  43.  305.) 

Green  modification.  Five  times  more  sol. 
than  ordinary  sublimed  sulphur  in  a  mixture 
of  salicylaldehyde  and  benzene.  (Orloff,  C.  C. 
1902,  I.  1264.) 

The  following  data  relate  to  octahedral  or 
ordinary  sulphur  (A.  1): — • 

Sol.  in  warm  liquid  H2S  (Niemann);  warm 
P2S3,  SBr2,  SC12,  Br2,  NC13,  BaS+Aq 
(Dumas);  in  alcoholic  solution  of  K2S5,  but 
is  repptd.  by  addition  of  H2O  to  sat.  solu- 
tion. 

Sol.  in  liquid  SO2. 

Sol.  in  aqueous  solution  of  alkali  sulphates, 
especially  when  hot.  SI.  sol.  in  boiling  cone. 
HSCN+Aq,  from  which  it  mostly  separates 
on  cooling. 

Na2CO3+Aq  (5.6%  Na2CO3)  dissolves  no 
S  at  20°;  0.06775%  at  100°.  (Pohl,  Dingl. 
197.  508.) 

The  solubility  9f  S  in  Na2S+Aq  between 
0°  and  50°  diminishes  slightly  with  increase 
in  temp.,  but  increases  with  dilution  of  the 
solution,  having  its  largest  value  in  a  N/16 
solution  of  Na2S-f  Aq  when  the  relation  of 
Na2S  to  dissolved  S  equals  about  1 : 4.  (Kiis- 
ter,  Z.  anorg.  1905,  43.  56.) 

Sol.  in  AlBr3.  (Isbekow,  Z.  anorg.  1913, 
84.  27.) 

Insol.  in  liquid  CO2.  (Biichner,  Z.  phys. 
Ch.  1906,  54.  674.) 

Sol.  in  liquid  NH3.  (Franklin,  Am.  Ch.  J. 
1898,  20.  822.) 

Sol.  in  liquid  NH3.  1  gr.  S  is  sol.  in  3-4 
ccm.  liquid  NH3.  (Hugot,  A.  ch.  1900,  (7)  21. 
32.) 

The  solubility  of  S  in  liquid  NH3  is  constant 
from— 23°  to— 84°  and  equals  39%.  (Ruff,  Z. 
angew.  Ch.  1910,  23.  1830.) 


Solubility  in  liquid  NH3. 
(g.  S  in  100  g.  solution.) 


t° 

S' 

t° 

S 

—78 
—20.5 
0 

38.6 
38.  T 
32.34 

16.4 
30 
40 

25.65 
21.0 
18.5 

(Ruff  and  Hecht,  Z.  anorg.   1911,  70.  62.) 

SI.  sol.  in  liquid  NO2.  (Frankland,  Chem. 
Soc.  1901,  79.  1361.) 

S2C12  dissolves  66.74%  S  at  ord.  temp,  to 
form  a  liquid  of  1.7  sp.  gr.  (Rose.) 

Solubility  of  S  in  S2C12  varies  according  to 
the  variety  of  sulphur  used.  Aten  has  pub- 
lished an  extended  investigation  on  the  sub- 
ject, which  see  for  details.  (Z.  phys.  Ch.  1905- 
14,  54.  86, 124;  81. 268;  83. 443;  86. 1;  88. 321.) 

Solubility  in  SnCl4. 

100  g.  SnCl4  dissolve  at: 
99°        101°       110°       110° 
5.8          6.2         8.7        9.1  pts.  solid  S, 

112°  112°  121° 

9.4  9.9  17.0  pts.  liquid  S. 

(Gerardin.) 

Sol.  in  alkalies +Aq  with  decomp. 
Sol.  in  1926.7  pts.  absolute  alcohol  at  15°. 
(Pohl,  W.  A.  B.  6.  600.) 

Sol.  in  20  pts.  hot  nearly  absolute  alcohol,  less  sol.  in 
weaker  alcohol.  (Laurogais.) 

Sol.  in  600  pts.  boiling  alcohol  of  40°  B.  (Chevallier, 
J.  ch.  med.  2.  587);  in  500  pts.  alcohol  (Meissner) ;  200 
pts.  alcohol  (Pelouze  and  Fremy). 

100  pts.  absolute  alcohol  dissolve  0.42  pt. 
at  b.-pt.,  and  0.12  pt.  S  at  16°;  100  pts.  ether 
dissolve  0.54  pt.  at  b.-pt.,  and  0.19  pt.  S  at 
16°;  100  pts.  benzene  dissolve  17.04  pts.  at 
b.-pt.,  and  1.79  pts.  S  at  16°;  100  pts.  oil  of 
turpentine  dissolve  16.16  pts.  at  b.-pt.,  and 
1.35  pts.  S  at  16°;  100  pts.  CS2  dissolve  73.46 
pts.  at  b.-pt.,  and  38.  70  pts.  S  at  16°;  100  pts. 
naphtha  dissolve  10.56  pts.  at  b.-pt.,  and 
2.77  pts.  S  at  16°;  100  pts.  tar-oil  dissolve 
26.98  pts.  at  b.-pt.,  and  1.51  pts.  S  at  16°. 
(Payen,  C.  R.  34.  456.) 

100  pts.  absolute  methyl  alcohol  dissolve 
0.028  pt.  at  18.5°;  100  pts.  absolute  ethyl 
alcohol  dissolve  0.053  pt.  at  18.5°.  (de 
Bruyn,  Z.  phys.  Ch.  10.  781.) 

Solubility  in  amyl  alcohol. 
95°         110°         110° 
1.5          2.1  2.2  pts.  solid  S, 

112°       112°       120°       131° 
2.6         2.7         3.0        5.3  pts.  liquid  S. 
(Gerardin,  A.  ch.  (4)  5.  134.) 

Quickly  sol.  in  12.5  pts.  ether.    (Favre.) 
100  pts.  benzene  dissolve  0.965  pt.  S  at  26°; 

100  pts.  benzene  dissolve  4.377  pts.  S  at  71°; 

100  pts.  toluene  dissolve  1.479  pts.  S  at  23°; 

100  pts.  ethyl  ether  dissolve  0.972  pt.  S  at 


896 


SULPHUR 


23.5°;  100  pts.  chloroform  dissolve  1.205  pts. 
S  at  22°;  100  pts.  phenol  dissolve  16.35  pts. 
S  at  174°;  100  pts.  aniline  dissolve  85.27  pts. 
S  at  130°.  (Cossa,  B.  1.  139.) 


Solubility  in  benzene  at  t°. 

—77°    —84.5°    —89°    —116° 
4.84        4.46         4.29          2.99  g.  S. 

(Arctowski,  Z.  anorg.  1896,  11.  274.) 
When  20  pts.  S  dissolve  in  50  pts.  CS 

t 

g.  S  in  10  g.  of  solution 

15.17 
19.29 

0.1480 
0.1692 

(Bronsted,  Z.  phys.  Ch.  1906,  55.  377.) 

A  mixture  of  S  and  toluene  separates  into 
two  layers,  containing  33  and  92.5%  S  re- 
spectively. (Haywood,  J.  phys.  Ch.  1897,  1. 


CS2  dissolves  0.35  'pt.  ordinary  sulphur; 
some  varieties  of  S,  however,  are  not  entirely 


2.99  g.  S  are  sol.  in  100  grams  CS2  at  — 116°. 
(Arctowski,  C.  R.  1895,  121.  124.) 
Solubility  in  CS2. 
100  g.  of  the  sat.  solution  contain  at: 


22°  the  temp,  is  lowered  5°.    (Cossa.) 

Sat.  solution  of  S  in  CS2  boils  at  55°. 
(Cossa.) 


Sp.  gr.  of  S  dissolved  in  CS2  at  15°. 
(Pts.  S  per  100  pts.  CS2.) 


sol.  in  CS2,  thus— 

Sp.  gr. 

Pts.  S 

Sp.  gr. 

Pts.  S 

Sp.  gr. 

Pts.  S 

Variety  of  Sulphur 

15 

^ 

^ 

W. 

s'p 

£o.£ 

1.271 
1.272 
1.273 
1.274 
1.275 
1.276 
1.277 
1.278 
1.279 
1.280 
1.281 
1.282 
1.283 
1.284 
1.285 
1.286 
1.287 
1.288 
1.289 
1.290 
1.291 
1.292 
1.293 
1.294 
1.295 
1.296 
1.297 
1.298 
1.299 
1.300 
1.301 
1.302 
1.303 
1.304 
1.305 
1.306 
1.307 
1.308 
1.309 
1.310 
1.311 

0.0 
0.2 
0.4 
0.6 
0.9 
1.2 
1.4 
1.6 
1.9 
2.1 
2.4 
2.6 
2.9 
3.1 
3.4 
3.6 
3.9 
4.1 
4.4 
4.6 
4.8 
5.1 
5.3 
5.6 
5.8 
6.0 
6.3 
6.5 
6.7 
7.0 
7.2 
7.5 
7.8 
8.0 
8.2 
8.5 
8.7 
8.9 
9.2 
9.4 
9.7 

1.312 
1.313 
1.314 
1.315 
1.316 
1.317 
1.318 
1.319 
1.320 
1.321 
1.322 
1.323 
1.324 
1.325 
1.326 
1.327 
1.328 
1.329 
1.330 
1.331 
.332 
.333 
.334 
.335 
.336 
.337 
.338 
.339 
.340 
.341 
.342 
.343 
1.344 
1.345 
1.346 
1.347 
1.348 
1.349 
1.350 
1.351 

9.9 
10.2 
10.4 
10.6 
10.9 
11.1 
11.3 
11.6 
11.8 
12.1 
12.3 
12.6 
12.8 
13.1 
13.3 
13.5 
13.8 
14.0 
14.2 
14.5 
14.7 
15.0 
15.2 
15.4 
15.6 
15.9 
16.1 
16.4 
16.6 
16.9 
17.1 
17.4 
17.6 
17.9 
18.1 
18.4 
18.6 
18.9 
19.0 
19.3 

.352 
.353 
.354 
.355 
.356 
.357 
.358 
.359 
.360 
.361 
.362 
.363 
.364 
.365 
.366 
.367 
.368 
.369 
.370 
.371 
.372 
.373 
.374 
.375 
.376 
.377 
1.378 
1.379 
1.380 
1.381 
1.382 
1.383 
1.384 
1.385 
1.386 
1.387 
1.388 
1.389 
1.390 
1.391 

19.6 
19.9 
20.1 
20.4 
20.6 
21.0 
21.2 
21.5 
21.8 
22.1 
22.3 
22.7 
23.0 
23.2 
23.6 
24.0 
24.3 
24.8 
25.1 
25.6 
26.0 
26.5 
26.9 
27.4 
28.1 
28.5 
29.0 
29.7 
30.2 
30.8 
31.4 
31.9 
32.6 
33.2 
33.8 
34.5 
35.2 
36.1 
36.7 
37.2 

Octahedral,  from  Sicily 
Crystallised   in    dry    way,    re- 
cently prepared 
Do.,  prepared  8  years 
Do.,  prepared  9  years 
Do.,  prepared  15  years     . 
Red  needles,  recently  prepared 
Soft  yellow,             do. 
Do.,  prepared  2  years 
Soft  red,  recently  prepared  . 
Do.,  prepared  5  years 
Flowers  of  sulphur 
Do.,  another  sample 
Roll  brimstone,  outside 
Do.,  inside 

0.335 

0.415 
0.33 

0^382 

oisie 

0.374 
0'351 

0.000 

0.029 
0.004 
0.020 
0.051 
0.023 
0.353 
0.157 
0.157 
0.181 
0.113 
0.234 
0.029 
0.073 

(Deville,  A.  ch.  (3)  47.  99.) 

The  pt.  insol.  in  CS2  is  sol.  in  hot  absolute 
alcohol,  crystallising  on  cooling;  less  sol.  in 
chloroform  or  ether.    (Deville.) 

100  pts.  pure  CS2  dissolve  pts.  S  at  t°. 

t°                 Pts.  S                  t°                    Pts.  S 

—11             16.54           22                 46.05 
-  6             18.75            38                 94.57 
0            23.99           48.5           146.21 
+  15            37.15            55               181.34 
18.5         41.65 

(Cossa,  B.  1.  138.) 

Neither  ordinary  stick  S  nor  flowers  of  S 
is  completely  sol.  in  CS2.     Pptd.  S  is  com- 
pletely sol.  in  5  pts.  CS2.     (Tittenger,  C.  C. 
1894,  II.  267.) 

(Mascagno,  C.  N.  43.  192.) 

SULPHUR 


897 


Sp.  gr.  of  S  dissolved  in  CS2  at  15°.    Water  a 

Solubility  in  organic  solvents. 

4°  =  1. 

Sat.  solution 

Solvent 

t° 

contains  %  S 

Sp.  gr. 

%  s 

Sp.  gr. 

%  s 

Sp.  gr. 

% 

CS2 

—61 

3.6 

1.2708 
1.2717 
1.2727 
1  .  2792 
1.2802 
1.2812 
1.2822 

0.0 
0.2 
0.4 
1.8 
2.0 
2.2 
2.4 

1.2736 
1.2745 
1.2755 
1.3096 
1.3105 
1.3115 
1.3125 

0.6 
0.8 
1.0 

8.0 
8.2 
8.4 
8.6 

1.2764 
1.2774 
1.2783 
1.3409 
1.3419 
1.3430 
1.3440 

1.2 

1.4 
1.6 
14.2 
14.4 
14.6 
14.8 

—55 
—19 
—18 
—17 
—13 
—11 
—11 

4.4 
10.6 
10.8 
11.5 
12.4 
13.3 
13.5 

1.2832 

2.6 

1.3135 

8.8 

1.3450 

15.0 

—  2 

17.2 

1.2842 

2.8 

1.3145 

9.0 

1.3460 

15.2 

+  3 

19.5 

1.2852 

3.0 

.3155 

9.2 

1.3471 

15.4 

9 

23.1 

1.2862 

3.2 

.3165 

9.4 

1.3481 

15.6 

11 

23.7 

1.2872 

3.4 

.3175 

9.6 

1.3491 

15.8 

14 

25.9 

1.2882 
1.2892 

3.6 
3.8 

.3185 
.3195 

9.8 
10.0 

1.3502 
1.3512 

16.0 
16.2 

17 
19 

27.2 
28.9 

1.2901 

4.0 

.3205 

10.2 

1.3522 

16.4 

• 

20 

28.5 

1.2911 

4.2 

.3215 

10.4 

1.3532 

16.6 

21 

29.7 

1.2921 

4.4 

.3226 

10.6 

1.3543 

16.8 

26 

33.4 

1.2930 

4.6 

.3236 

10.8 

1.3553 

17.0 

27 

34.6 

1.2940 

4.8 

.3246 

11.0 

1.3563 

17.2 

29 

37.8 

1  .  2949 

5.0 

.3256 

11.2 

1.3573 

17.4 

30.5 

39.7 

1.2959 

5.2 

1.3266 

11.4 

1.3584 

17.6 

33 

42.2 

1.2969 

5.4 

1.3277 

11.6 

1.3594 

17.8 

40 

48.7 

1.2978 

5.6 

1.3287 

11.8 

1.3604 

18.0 

44 

53.2 

1  .  2988 

5.8 

1.3297 

12.0 

1.3615 

18.2 

46 

56.2 

1.2998 

6.0 

1.3307 

12.2 

1.3625 

18.4 

48 

57.5 

1.3008 

6.2 

1.3317 

12.4 

1.3635 

18.6 

• 

53 

60.0 

1.3017 

6.4 

1.3328 

12.6 

1.3646 

18.8 

54 

60.6 

1.3027 

6.6 

1.3338 

12.8 

1.3656 

19.0 

65 

67.9 

1.3037 

6.8 

1.3348 

13.0 

1.3667 

19.2 

77.5 

76.4 

1.3047 

7.0 

1  .  3358 

13.2 

1.3677 

19.4 

81.0 

79.4 

1.3056 
1  3066 

7.2 
7  4 

1.3368 
1  .  3379 

13.4 
13.6 

1.3688 
1  3698 

19.6 
19  8 

92.0 
98.0 

87.8 
90.1 

1.3076 

7.6 

1.3389 

13^8 

L3709 

2o!o 

Ethylene  dibromide 

9 

1.7 

1.3086 

7.8 

1  .  3399 

14.0 

22 

2.4 

40 

4.4 

(Pfeiffer,  Z.  anorg.  1897,  16.  200.) 

50 

72 

6.'4 
12.4 

Sol.  in  acetone.    (Eidmann,  C.  C.  1899,  II. 
1014.) 

. 

95 

108 

30.2 
60.0 

Benzene 

8 

1.2 

10 

1.3 

21 

1.8 

Solubility  of  S  in  acetone  +Aq  at  25°. 

30 

2.'e 

S  ==millimols.  g.  S  in  100  cc.  of  the  solution. 

39 

47 

3.3 
4r\ 

A  =  g.  acetone  in  100  g.  ace  tone  +Aq. 

rtl 

54 

f*K 

.  u 
4.9 

6Q 

A 

s 

Sp.  gr. 

DO 

72 

.8 
8.6 

100 

65.0 

0.78540 

100 
123 

17.5 

Q1     Q 

95.36 

45.0 

0.79114 

127 

OJ.  .  t/ 

34  0 

90.62 

33.0 

0.81654 

150 

Orr  .  \J 

36  8 

85.38 

25.3 

0.82958 

OU  .  o 

Hexane 

—20 

0.07 

(Herz  and  Knoch,  Z.  anorg.  1905,  46.  263.) 

0 
+26 

0.16 
0.41 

+68 

1.2 

+  130 

5.2 

+  142 

6.2 

+  184 

8.3 

(Etard,  A.  ch.  1894,  (7)  2.  571.) 

SULPHUR 


Solubility  in  CHC13  at  t°. 

t°                             g.  S  in  10  g.  of  solution 

12.25                             0.0744 
19.29                             0.0918 

(Bronsted,  Z.  phys.  Oh.  1906,  65.  377.) 

Solubility  of  octahedral  and  prismatic  S  in 
organic  solvents  at  t°. 

Solvent 

t° 

•     %    •     c, 

pnsmatic  b 

°7 
octahedral  S 

Benzene 

18.6 
25.3 

2.004 
2.335 

1.512 
1.835 

Chloroform 

0 
15.5 
40 

1.101 
1.658 
2.9 

0.788 
1.253 
2.4 

Ethyl  ether 

0 
25.3 

0.113 
0.253 

0.080 

a.  200 

Ethyl  bromide 

0 
25.3 

0.852 
1.676 

0.611 
1.307 

Ethyl  formate 

0 

0.028 

0.019 

Ethyl  alcohol 

25.3 

0.066 

0.052 

(Bronsted,  Z.  phys.  Ch.  1906,  55.  377.) 

Solubility  in  organic  solvents  at  25°.    (G.  S 
dissolved  in  1  g.  mol.  of  solvent.) 


Solvent 

g.  s 

Ethylene  chloride 
Tetrachlorethane 
Dichlorethylene 
Pentachlorethane 
Trichlorethylene 
Perchlorethylene 
Carbon  tetrachloride 

0.831 
2.063 
1.237 
2.421 
2.43 
2.537 
1  .  354 

(Hoffmann  et  al.  1910,  B.  43.  188.) 

100  g.  trichlorethylene  dissolve  1.19  g.  S 
at  15°.  (Wester  and  Bruins,  Pharm.  Weekhl 
1914,  51.  1443.) 

Solubility  in  benzyl  chloride  at  t°. 


t° 

g.  S  per  100  g.  of  solution 

in  upper  layer 

in  lower  layer 

0 

0.99 

17 

1.78 

35 

2.57 

46.1 

3.64 

63.3 

6.15 

78.0 

9.88 

99.1 

19.89 

109.6 

90.62 

114.6 

87.99 

118.8 

37!  29 

121.4 

40.04 

85  .'62 

130.0 

49.71 

80.07 

134.2 

56.20 

72.23 

Above    134.2°    sulphur    is    miscible    with 

Benzyl  chloride  in  all  proportions;  below  this 
;emp.  tAvo  layers  are  formed. 
(Bogusky,  J.  Russ.  Phys.  Chem.  Soc.  1905, 
37.  92-99;  C.  C.  1906,  I.  1207.) 

Easily  sol.  in  boiling  acetic  anhydride. 
(Rosenfeld,  B.  13.  1475.) 

Sol.  in  considerable  amount  in  warm  cone. 
HC2H3O2+Aq,  but  very  si.  sol.  if  dil.  (Lie- 
bermann,  B.  10.  866.) 

Sol.  in  stearic  acid+Aq.  (Vulpius,  Arch. 
Pharm.  (3)  13.  38.) 

Acetic  ether  dissolves '6%  S.    (Favre.) 

Difficultly  sol.  in  methyl  acetate.  (Nau- 
mann,  B.  1909,  42.  3790.) 

Sol.  in  ethyl  acetate.  (Naumann,  B.  1904, 
37.  3601.) 

SI.  sol.  in  benzonitrile  at  ord.  temp.,  much 
more  sol.  at  higher  temp.  (Naumann,  B. 
1914,  47.  1369.) 

Sol.  in  12  pts.  hot  petroleum  from  Amiano, 
but  nearly  insol.  in  cold,  (de  Saussure.) 

100  pts.  nicotine  at  100°  dissolve  10.58  pts. 
S,  but  this  separates  out  as  the  solution  cools. 
(Kiever,  C.  C.  1872.  434.) 

Sol.  in  warm  aniline.  (Barral,  A.  ch.  (3) 
20.  352.) 

Easily  sol.  in  hot,  less  sol.  in  cold  aniline. 
(Fritzsche.) 

Very  sol.  in  aniline  and  quinoline,  especially 
when  warm.  (Hofmann.) 

Sol.  in  quinoline  but  reacts  with  the  solvent 
with  evolution  of  H.  (Beckmann  and  Gabel, 
Z.  anorg.  1906,  51.  236.) 

l/z  ccm.  oleic  acid  dissolves  0.0335  g.  S  in 
6  days.  (Gates,  J.  phys.  Chem.  1911,  15. 
143.) 

Sol.  in  2.6  pts.  of  boiling,  si.  sol.  in  cold 
creosote. 

Sol.  by  digestion  in  2  pts.  oil  of  turpentine. 

Sol.  in  hot  oil  of  copaiba,  crystallising  on 
cooling. 

Sol.  in  hot  oil  of  mandarin,  crystallising 
on  cooling. 

Sol.  in  hot  oil  of  caraway,  crystallising  on 
cooling. 

Somewhat  sol.  in  hot,  less  in  cold  wood- 
spirit. 

SI.  sol.  in  lignone,  bromoform,  cold  ben- 
zene, but  easily  in  hot  benzene.  (Mansfield, 
Chem.  Soc.  1/262.) 

Sol.  in  ethyl  sulphide,  and  carbon  chlo- 
ride. (Rathke,  A.  152.  187.) 

Sol.  in  mercuric  methyl. 

Sol.  in  20  pts.  ethyl  nitrate,  from  which  is 
is  not  pptd.  by  H2O. 

Sol.  in  naphtha,  aldehyde,  ipdal,  bromal, 
chloroform,  warm  chloral,  sinkaline+Aq, 
ethyl  chloride,  warm  benzoyl  chloride. 

100  pts.  methylene  iodide  dissolve  10  pts 
S  at  10°.  Melted  sulphur  is  miscible  with 
hot  methylene  iodide.  (Retgers,  Z.  anorg 
3.  343.)  ' 

S  dissolves  in  2000  pts.  glycerine.  (Caj 
and  Garot,  J.  Pharm.  (3)  26.  81.) 

Glycerine  dissolves  0. 10 %  S.  (Kiever,  C.  C 
1872.  434.) 


SULPHUR  CHLORIDE  AMMONIA 


899 


100  g.  glycerine  dissolve  0.14  g.  at.  15.5°. 
(Ossendowski,  Pharm.  J.  1907,  79.  575.) 

Sol.  in  butyl  sulphydrate,  and  warm  retin- 
ole. 

Sol.  in  ethyl  sulphydrate. 

Very  sol.  in  coniine,  hexyl  alcohol,  warm 
allyl  sulphocyanide,  cacodyl  oxide.  Some- 
what sol.  in  hot  styrene,  separating  out  on 
cooling. 

Readily  sol.  in  warm,  less  readily  in  cold 
toluene  or  resin-oil. 

Sol.  in  olive  oil  at  115°,  from  which  it 
mostly  separates  on  cooling. 

Sol.  in  hot  oil  of  amber,  crystallising  upon 
cooling.  Sol.  in  2  pts.  hot,  si.  sol.  in  cold 
caoutchin. 

Insol.  in  yalerianic  acid,  amyl  valerate, 
valeryl  hydride. 

Linseed  oil  dissolves  %  S  at  t°. 


t° 

%  s 

t° 

%s  . 

t? 

%s 

25 

0.630 

95 

2.587 

160 

9.129 

60 

1.852 

130 

4.935 

(Pohl.) 

Solubility  in  olive  oil  (sp.  gr.  =0.885). 
100  pts.  dissolve  pts.  S  at  t°. 


t° 

Pts.  S 

t 

Pts.  S 

t° 

Pts.  S 

15 

2.3 

65 

20.6 

110 

30.3 

40 

5.6 

100 

25.0 

130 

43.2 

(Pelouze,  C.  H.  68.  1179.) 
Solubility  in  100  pts.  coal-tar  oil  at  t°. 


Pts.  S  in 

t° 

Oil  of  0.870 

Oil  of  0.880 

Oil  of  0.882 

sp.  gr. 

sp.  gr. 

sp.  gr. 

--!.'•':':  .iG 

B.-pt.  80-100° 

B.-pt.  85  120° 

B.-pt.  120-200° 

15 

2.1 

2.3 

2.5 

30 

3.0 

4.0 

5.3 

50 

5.2 

6.1 

8.3 

80 

11.8 

13.7 

15.2 

100 

15.2 

18.7 

23.0 

110 

23.0 

26.2 

120 

27.0 

32.0 

130 

38.7 

Pts.  S  in 

Oil  of  0.885 

Oil  of  1.010 

Oil  of  1.020 

sp.  gr.  B.-pt. 
150  200° 

sp.  gr.  B.-pt. 
210300° 

sp.  gr.  B.-pt. 

220-300° 

15 

2.6 

6.0 

7.0 

30 

5.8 

8.5 

8.5 

50 

8.7 

10.0 

12.0 

80 

21.0 

37.0 

41.0 

100 

26.4 

52.5 

"54.0 

110 

31.0 

105.0 

115.0 

120 

38.0 

00 

oo 

130 

43.8 

00 

00 

(Pelouze,  C.  R.  69.  56.) 

Sulphur  bromide,  S2Br2. 

Decomp.  gradually  with  H2O.  Dissolves  S 
on  warming,  which  crystallises  out  on  cooling. 
Sol.  in  CS2. 

Decomp.  by  current  of  dry  air  into  S  and 
Br.  (Hannay,  Chem.  Soc.  36.  16.) 

Decomp.  slowly  by  cold  H2O,  rapidly  by 
hot  H2O.  Decomp.  by  dil.  KOH+Aq  or 
NaHCO3+Aq.  (Korndorfer,  Arch.  Pharm. 
1904,  242.  156.) 

A  study  of  the  mpt.  curve  of  a  series  of 
mixtures  of  sulphur  and  bromine  gave  no 
evidence  for  the  existence  of  the  compounds 
SBr2  and  SBr4.  (Ruff,  B.  1903,  36.  2446.) 

Sulphur  racwochloride,  S2C12. 

Slowly  decomp.  by  H2O.  Miscible  with 
CS2  and  C6H6.  Sol.  in  alcohol  and  ether  with 
subsequent  decomposition.  Sol.  in  oil  of  tur- 
pentine. 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  830.) 

Sol.  in  CC14,  and  C6H6.  (Oddo,  Gazz.  ch. 
it.  1899,  29.  (2)  318.) 

Sulphur  ^'chloride,  SC12. 

Decomp.  slowly  with  H2O,  immediately  by 
alcohol  or  ether. 

Sulphur  tefrachloride,  SC14. 

Violently  decomp.  by  H2O.  Decomp.  at 
temperatures  above  — 22°.  (Michaelis,  A. 
170.  1.) 

Sulphur  stannic  chloride,  2SC14,  SnCl4. 

Decomp.  by  H2O.  Sol.  in  dil.  HNO3+Aq. 
Forms  a  mass  with  fuming  HNO3  which  is 
sol.  in  HNO3+Aq.  Sol.  in  POC13.  (Cassel- 
mann.) 

Very  hydroscppic.  Fumes  in  moist  air. 
Very  easily  sol.  in  dry  abs.  ether  and  in  ben- 
zene. Sol.  in.CHCla,  SO2C12,  CS2,  POC13 
ligroin  and  petroleum  ether.  (Ruff,  B.  1904, 
37.  4517.) 

Sulphur  titanium  chloride,  SC14,  2TiCl4. 

Very  deliquescent.  Easily  sol.  in  dil. 
HNOs+Aq.  (Weber,  Pogg.  132.  454.) 

SC14,  TiCl4.  Sol.  in  SO2C12,  CHC13,  CS2 
and  petroleum  ether.  (Ruff,  B.  1904,  37. 
4516.) 

Sulphur  chloride  ammonia,  S2C12,  4NH3. 

Insol.  in  H2O,  but  gradually  decomp. 
thereby;  sol.  without  decomp.  in  absolute 
alcohol,  from  which  it  is  pptd.  by  H2O. 
(Mertens.) 

Does  not  exist.  (Fordos  and  Gelis,  C.  R. 
31.  702.) 

SC12,  2NH3.  Decomp.  by  H2O.  Sol.  in 
alcohol  or  ether.  (Soubeiran,  A.  ch.  67.  71.) 
Not  a  true  chemical  compound,  but  a  mixture. 
(Fordos  and  Gelis,  C.  R.  31.  702.) 


900 


SULPHUR  CHLORIDE  NITROGEN  SULPHIDE 


SC12,  4NH3.  Decomp.  by  H2O.  SI.  sol.  in 
absolute  alcohol  and  ether  (Soubeiran,  A.  ch. 
67.  71);  mixture  (Fordos  and  Gelis). 

Sulphur  chloride  nitrogen  sulphide. 
See  Nitrogen  sulphochloride. 


Sulphur  perfluoride,  SF6. 

Very  si.  sol.  in  H2O;  si.  sol.  in 
(Moissan,  C.  R.  1900,  130.  868.) 


alcohol. 


Sulphur  monoiodide,  S2l2. 

Insol.  in  H2O.  Decomp.  by  alcohol,  which 
dissolves  out  I2.  SI.  sol.  in  cold  caoutchin, 
the  solution  decomposing  when  boiled.  Freely 
sol.  in  glycerine.  Sol.  in  60  pts.  glycerine, 
and  82  pts.  olive  oil.  (Cap  and  Garot,  J. 
Pharm.  (3)  26.  81.) 

Very  sol.  in  liquid  NH3.  (Franklin,  Am. 
Ch.  J.  1898,  20.  830.) 

Sol.  in  CS2.  (Linebarger,  Am.  Ch.  J.  1895, 
17.  58.) 

Sulphur  Aeododide,  SI6. 

Decomp.  on  air.  Alcohol  or  alkalies  dis- 
solve out  iodine,  (vom  Rath,  Pogg.  110.  116.) 

Does  not  exist.  (M'Leod,  Rep.  Brit.  Assn. 
Advn.  Sci.  1892.  690.) 

Sulphur  stannic  iodide. 
See  Tin  sulphur  iodide. 

Sulphur  sesgwioxide,  S2O3. 

Deliquescent.  Violently  decomp.  by  H20 
at  ordinary  temp.  Sol.  in  fuming  H2SO4.  In- 
sol. in  SO 3.  Decomp.  by  alcohol  or  other. 
(Weber,  Pogg.  166.  531.) 

Sulphur  dioxide,  SO2. 

Liquid.  Insol.  in  H2O  if  brought  in  con- 
tact therewith  below  the  b.-pt.  of  S02. 

Sol.  in  3  yols.  CS2  on  warming,  separating 
out  on  cooling.  Dissolves  some  P,  little  S, 
and  no  sulphuric  or  phosphoric  acids. 

Dissolves  ether,  chloroform,  P,  Br,  S,  I, 
CS2,  colophonium,  and  other  gums;  also 
benzene  when  warmed.  (Sestini,  Bull.  Soc. 
(2)  10.  226.) 

Miscible  with  liquid  SO3,  but  not  with 
H2S04. 

Gas. 

1  vol.  H2O  absorbs  30  vols.  SO2  gas  at  18°  (Davy) ;  20 
vols.  at  ord.  temp.  (Dalton) ;  43.78  vols.  at  ord.  temp, 
(de  Saussure) ;  50  vols.  at  20°  and  760  mm.  (Pelouze  and 
Fremy) ;  33  vols.  at  ord.  temp.  (Thomson) . 

1  pt.  SO2  (by  wtight)  is  sol.  in  0.1429  pt.  H2O  at  5°, 
and  the  solution  has  1.020  sp.  gr. 

1  pt.  SO i  is  sol.  in  0.0400  pt.  H2O  at  ord.  temp. 
(Priestley) ;  in  0.0909  pt.  H  O  at  16°,  and  sp.  gr.  of  the 
solution  =  1.05 13  (Thomson). 

Sol.  in  2  pts.  HiO  at  10°.    (Pierre,  A.  ch.  (3)  23.  421.) 

100  vols.  H2O  at  18°  and  760  mm.  absorb  4378  vols. 
SO2  gas;  100  vols.  alcohol  of  0.84  sp.  gr.  at  760  mm. 
absorb  11,577  vols.  (de  Saussure,  1814.) 


Solubility  of  SO2  gas  in  H2O.  t°  =  temp. ;  V  = 
vols.  SO2  reduced  to  0°  and  760  mm.  con- 
tained in  1  vol.  sat.  SO2+Aq;  Vi=vols. 
SO2  gas  reduced  to  0°  and  760  mm.  dis- 
solved by  1  vol.  H2O  under  760  mm.  pres- 
sure. 


t° 

V 

Vi 

t° 

V 

Vi 

0 

68.861 

79.789 

21 

34.986 

37.970 

1 

67.003 

77.210 

22 

33.910 

36.617 

2 

65.169 

74.691 

23 

32.847 

35.302 

3 

63.360 

72.230 

24 

31.800 

34.026 

4 

61.576 

69.828 

25 

30.766 

32.786 

5 

59.816 

67.485 

26 

29.748 

31.584 

6 

58.080 

65.200 

27 

28.744 

30.422 

7 

56.369 

62.973 

28 

27.754 

29.314 

8 

54.683 

60.805 

29 

26.788 

28.210 

9 

53.021 

58.697 

30 

25.819 

27.161 

10 

51.383 

56.647 

31 

24.873 

26.151 

11 

49.770 

54  .  655 

32 

23.942 

25.178 

12 

48.182 

52.723 

33 

23.025 

24.244 

13 

46.618 

50.849 

34 

22.122 

23  .  347 

14 

45.079 

49.033 

35 

21.234 

22.489 

15 

43.564 

47.276 

36 

20.361 

21.668 

16 

42.073 

45.578 

37 

19.502 

20.886 

17 

40.608 

43  .  939 

38 

18.658 

20.141 

18 

39.165 

42.360 

39 

17.827 

19.435 

19 

37  .  749 

40.838 

40 

17.013 

18.766 

20 

36.206 

39.374 

(Schonfeld,  A.  96.  5.) 


This  table  may  be  formulated  as  follows: 
1  vol.  H2O  absorbs  79. 789-2. 6077t+ 
0.029349t2  vols.  SO2  at  temp,  between  0°  and 
20°,  or  1  vol.  sat.  solution  contains  68.861— 
1.87025t+0.01225t2  vols.  SO2.  Coefficient  of 
absorption  between  21°  and  40°  =  75. 182— 
2.1716t+0.01903t2  vols.  SO2  or  1  vol.  sat. 
solution  between  21°  and  40°  contains  60.952 
— 1.38898t+0.00726t2  vols.  SO2. 


Solubility  of  SO2  in  H2O  at  various  temps,  and 
760  mm.  t°  =  temp.;  G  =  grammes  SO2 
dissolved  in  1  g.  H2O;  V  =  vols.  SO2  dis- 
solved in  1  g.  H2O. 


t° 

G 

V 

t° 

G 

V 

8 

0.168 

58.7 

30 

0.078 

27.3 

10 

0.154 

53.9 

32 

0.073 

25.7 

12 

0.142 

49.6 

34 

0.069 

24.3 

14 

0.130 

45.6 

36 

0.065 

22.8 

16 

0.121 

42.2 

38 

0.062 

21.6 

18 

0.112 

39.3 

40 

0.058 

20.4 

20 

0.104 

36.4 

42 

0.055 

19.3 

22 

0.098 

34.2 

44 

0'.053 

18.4 

24 

0.092 

32.3 

46 

0.050 

17.4 

26 

0.087 

30.5 

48 

0.047 

16.4 

28 

0.083 

28.9 

50 

0.045 

15.6 

(Sims,  A.  118.  340.) 


SULPHUR  OXIDE 


901 


Solubility  of  SO2  in  H2O  at  various  pressures. 
P  =  "partial  pressure,"  i.e.  the  total  pres- 
sure minus  the  tension  of  aqueous  vapour 
at  given  temp.;  G  at  P  =  weight  SO2  in 
grammes,  which  is  dissolved  in  1  g.  H2O 
.at  pressure  P;  G  at  760  =  calculated 
weight  SO  2  that  would  be  contained  in 
1  g.  H2O  at  760  mm.  if  the  absorption  were 
proportional  to  the  pressure;  V  =  the 
volume  of  G  grammes  of  SO2  at  0°  and 
760  mm. 


P 

7° 

GatP 

G  at  760 

VatP 

V  at  760 

30 

0.010 

0.263 

3.634 

92.06 

40 

0.013 

0.242 

4.451 

84.55 

50 

0.015 

0.223 

5.129 

77.95 

60 

0.017 

0.818 

6.024 

76.28 

70 

0.020 

0.213 

6.868 

74.55 

80 

0.022 

0.210 

7.743 

73.55 

90 

0.025 

0.208 

8.598 

72.62 

100 

0.027 

0.205 

9.421 

71.60 

120 

0.032 

0.201 

11.09 

70.20 

140 

0.036 

0.197 

12.71 

69.00 

160 

0.041 

0.195 

14.34 

68.15 

180 

0.046 

0.193 

15.97 

67.40 

200 

0.050 

0.191 

17.59 

66.83 

220 

0.055 

0.190 

19.19 

66.30 

240 

0.059 

0.188 

20.79 

65.84 

260 

0.064 

0.187 

22.40 

65.44 

280 

0.069 

0.186 

23.99 

65.10 

300 

0.073 

0.185 

25.59 

64.81 

350 

0.085 

0.184 

29.55 

64.16 

400 

0.096 

0.182 

33.51 

63.65 

450 

0.107 

0.181 

37.44 

63.25 

500 

0.118 

0.180 

41.42 

62.94 

550 

0.130 

0.179 

45.31 

62.60 

600 

0.141 

0.178 

49.20 

62.32 

650 

0.152 

0.178 

53.10 

62.09 

700 

0.163 

0.177 

56.98 

61.86 

750 

0.174 

0.176 

60.88 

61.69 

760 

0.176 

0.176 

61.65 

61.65 

800 

0.185 

0.176 

64.74 

61.50 

850 

0.196 

0.175 

68.57 

61.30 

900 

0.207 

0.175 

72  .41 

61.15 

950 

0.218 

0.175 

76.25 

61.00 

1000 

0.229 

0.174 

80.01 

60.88 

1050 

0.240 

0.174 

83.97 

60.77 

1100 

0.251 

0.174 

87.80 

60.65 

1200 

0.273 

0.173 

95.45 

60.45 

1300 

0.295 

0.172 

103.00 

60.25 

20° 

P 

GatP 

G  at  760 

Vat  P 

V  at  760 

40 

0.007 

0.143 

2.637 

50.09 

50 

0.009 

0.138 

3.171 

48.20 

60 

0.011 

0.135 

3.718 

47.10 

70 

0.012 

0.131 

4.205 

45.64 

80 

0.013 

0.127 

4.663 

44.30 

90 

0.015 

0.125 

5.169 

43.65 

100 

0.016 

0.124 

5.692 

43.25 

120 

0.019 

0.121 

6.683 

42.33 

140 

0.022 

0.119 

7.690 

41.75 

160 

0.025 

0.118 

8.666 

41.17 

180 

0.028 

0.117 

9.652 

40.75 

200 

0.030 

0.116 

10.62 

40.35 

220 

0.033 

0.115 

11.59 

40.03 

240 

0.036 

0.114 

12.54 

39.70 

260 

0.038 

0.112 

13.45 

39.30 

280 

0.041 

0.112 

14.41 

39.10 

300 

0.044 

0.111 

15.34 

38.87 

350 

0.050 

0.110 

17.66 

38.35 

400 

0.059 

0.109 

20.56 

38.10 

450 

0.064 

0.108 

22.37 

37.77 

500 

0.071 

0.107 

24.67 

37.50 

550 

0.077 

0.106 

26.93 

37.20 

600 

0.083 

0.105 

29.14 

36.90 

650 

0.090 

0.105 

31,39 

36.70 

700 

0.096 

0.105 

33.62 

36.50 

750 

0.103 

0.104 

35.94 

36.43 

760 

0.104 

.  0.104 

36.43 

36.43 

800 

0.110 

0.104 

38.32 

36.40 

1000 

0.137 

0.104 

47.85 

36.37 

1300 

0.178 

0.104 

62.10 

36.31 

1600 

0.218 

0.104 

76.35 

36.27 

1900 

0.259 

0.104 

90.53 

36.21 

39.8° 

P 

G  at  P 

G  at  760 

Vat  P 

V  at  760 

200 

0.016 

0.062 

5.675 

21.57 

300 

0.024 

0.061 

8.368 

21.20 

400 

0.031 

0.060 

11.03 

20.95 

500 

0.039 

0.059 

13.67 

20.77 

600 

0.047 

0.059 

16.29 

20.64 

760 

0.059 

0.059 

20.50 

20.50 

800 

0.062 

0.059 

21.58 

20.50 

1000 

0.077 

0.058 

26.84 

20.40 

1500 

0.113 

0.057 

39.65 

20.09 

2000 

0.149 

0.057 

52.11 

19.80 

50° 

P 

GatP 

G  at  760 

VatP 

V  at  760 

200 

0.012 

0.045 

4.156 

15.97 

400 

0.024 

0.015 

8.275 

15.72 

600 

0.035 

0.045 

12.36 

15.65 

760 

0.045 

0.045 

15.62 

15.62 

800 

0.047 

0.045 

16.43 

15.60 

1000 

0.059 

0.045 

20.51 

15.59 

1500 

0.088 

0.044 

30.73 

15.57 

2000 

0.012 

0.044 

39.07 

15.55 

(Sims?  A.  118.340.) 

902 


SULPHUR  OXIDE 


1  g.  H2O  dissolves  0.0909  g.  SO2  =  34.73  cc. 
(at  25°)  at  25°  and  748  mm.  pressure.    (Wai- 
den  and  Centnerszwer,  Z.  phys.  Ch.  1901,  42. 
462.) 

Solubility  of  SO2  in  H2O  at  t°  and  760  mm. 
pressure. 

Sp.  gr.  of  SOa+Aqat  4°. 

& 

Sp.  gr. 

% 
S02 

Sp.  gr. 

& 

Sp.  gr. 

\ 

2 
3 
4 
5 
6 
7 

1.0024 
1  .  0049 
1.0075 
1.0102 
1.0130 
1.0158 
1.0187 

8 
9 
10 
11 
12 
13 
14 

1.0217 
1.0247 
1.0278 
1.0311 
1.0343 
1.0376 
1.0410 

15 

16 
17 
18 
19 
20 
21 

1.0445 
1.0480 
1.0517 
1.0553 
1.0591 
1.0629 
1.0667 

t° 

G.  SO2  per 
1  g.  H20 

t° 

G.  S02  per 
1  g.  H20 

0 
2 
4 
6 

0.236 
0.218 
0.201 
0.184 

7 
8 
10 
12 

0.176 
0.168 
0.154 
0.142 

(Schiff,  calculated  by  Gerlach,  Z.  anal.  8.  292.) 

(Roozeboom,  R.  t.  c.  1884,  3.  29.) 

From  a  gas  containing  10%  by  vol.  of  SO2 
at  10°  1.63%  by  wt.  is  dissolved  by  1  litre 
of  H2O;  if  the  pressure  is  increased  to  5  at- 
mospheres, 8.14%  by  wt.  is  dissolved. 
(Harpf,  Chem.  Zeitschr.,  1905,  4.  136.) 

Solubility  of  SO2  in  H2O  at  t°. 
C  =  g.  SO2  in  1  cc.  of  the  solution. 
P  =  Pressure  in  mm.  of  Hg. 


t° 

C 

p 

|xW 

0 

0.000537 
0.00237 
0.01227 
0.03894 

0.4 
3.5 
29.4 
109.4 

13.4 

6.78 
4.17 
3.48 

25 

0.000534 
0.00234 
0.01212 
0.03750 

1.4 
11.75 

87.9 
313.0 

3.81 
2.00 
1.379 
1.198 

50 

u 
(I 

a 

0.000525 
0.002276 
0.01181 
0.03628 

4.9 
30.5 
204.5 
696.0 

1.07 
0.746 
0.577 
0.521 

(Lindner,  M.  1912,  33.  645.) 

Sp.  gr.  of  sat.  solution  at — 

0°  10°  20°  40° 

1.06091     1.05472     1.02386     0.95548 
(Bunsen  and  Schonfeld,  A.  95.  2.) 

Sat.  S02+Aq  has  sp.  gr.  =  1.0040.     (Ber- 
thollet.) 

Sp.  gr.  of  sat.  SO2+Aq  at  t°. 


t° 

Sp.  gr. 

t° 

Sp.  gr. 

t° 

Sp.  gr. 

0 

1.0809 

9 

.0548 

17 

1.0358 

1 

1.0596 

10 

.0547 

18 

.0321 

2 

1.0585 

11 

.0528 

19 

.0281 

3 

1.0576 

12 

.0505 

20 

.0239 

4 

1.0569 

13 

.0481 

21 

.0195 

5 

1.0562 

14 

.0454 

22 

1.0147 

6 

1.0557 

15 

.0424 

23 

1.0099 

7 

1.0552 

16 

.0392 

24 

0.9991 

8 

1.0549 

Sp.  gr.  of  SO2+Aq. 


(Schiff,  A.  107.  312.) 


%S02 

Temp. 

Sp.  gr. 

0.99 
2.05 
2.87 
4.04 
.     4.99 
5.89 
7.01 
8.08 
8.68 
9.80 
10.75 
11.65 
13.09 

15.5° 

12.5° 
11.0° 

1.0051 
.0102 
.0148 
.0204 
.0252 
.0297 
.0353 
.0399 
.0438 
.0492 
.0541 
.0597 
1.0668 

(Giles  and  Schearer,  Jour.  Soc.  Ch.  Ind.  4. 
303.) 

Sp.  gr.  of  SO2+Aq. 

% 
S02 

Sp.  gr. 

& 

Sp.  gr. 

s%2     SP-  gr- 

1 

2 
3 

1.0052 
1.0094 
1.0134 

4 
5 

6 

1.0167 
1.0208 
1.0242 

7       1.0283 
8       1.0329 
9       1.0402 

(Anthon.) 
Sp.  gr.  of  SO2+Aq. 

s76, 

Sp.  gr. 

% 
SO2 

Sp.  gr. 

&       Sp.g, 

1 

2 
3 

4 

1.0042 
1.0083 
1.0125 
1.0167 

5 

; 

1.0210 
1.0252 
1.0295 

8      1.0348 
9       1.0392 
10      1  .  0438 

(Hager,    Adjumenta    varia,    Leipzig,    1876. 
146.) 

SULPHUR  OXIDE 


903 


Sp.  gr.  of  SO2+Aq  at  15°. 

Solubility  of  SO2  in  H2SO4  of  1.84  sp.  gr. 

s76, 

Sp.  gr. 

s^ 

Sp.  gr. 

$,. 

Sp.  gr. 

t° 

fll 

a^,  a 

CO  O'o 

GO 

all 

d&6 
§i§ 
°ife 

t° 

III 

£<o1 

GO 

rfl 

^  o  o 

0.5 
1.0 
1.5 
2.0 
2.5 
3.0 
3.5 

1.0028 
1.0056 
1.0085 
1.0113 
1.0141 
1.0168 
1.0194 

4.0 
4.5 
5.0 
5.5 
6,0 
6.5 
7.0 

1.022.1 
1.0248 
1.0275 
1.0302 
1,0328 
1.0353 
1.0377 

7.5 

8.0 
8.5 
9.0 
9.5 
10.0 

1.0401 
1.0426 
1.0450 
1.0474 
1.0497 
1  .  0520 

0 
10 
20 
25 
30 
40 

L8232 
1.8225 
1.8221 
1.8216 
1.8205 

53 
35.0 
25.0 
21.0 
18.0 
13.0 

50 
60 
70 
80 
90 

1.8186 
1.8165 
1.8140 
1.8112 
1.8080 

9.5 
7.0 
5.5 
4.5 
4.0 

(Scott,  Polyt.  Centralbl.  1873.  826.) 

Cone.  H2SO4  absorbs  0.009  pt.  by  weight 
(58  vols.),  and  SO2  is  more  soluble  in  dilute 
H2SO4-fAq,  the  more  H20  there  is  present. 
(Kolb,  Dingl.  209.  270.) 

Solubility  in  H2SO4. 

(Dunn,  C.  N.  1882,  45.  272.    Calc.  by  Seidell, 
Solubilities,  1st  Ed.) 

Solubility  of  SO2  in  H2SO4+Aq. 

t° 

4! 

aE  2 
•a-gg 

P 
^ 

il 

ttB 

31 

t 

•  o  o 
B&J 
dKj2 
M^° 

g? 

lw 
££? 

oj 

It 

Sp.  gr.  of 
H;S04 

Absorbs  SO  2 
per  kg. 

Absorbs  SO  2 
per  litre 

1 
;:  -1 
1 
1 
I 
1 

.841 
.839 
.540 
.407 
.227 
.020 

0.009 
0.014 
0.021 
0.032 
0.068 
0.135 

5.8 
8.9 
11.2 
15.9 
29.7 
49.0 

6.9 
6.9 
8.6 
9.8 
5.5 
6.6 

1.139 
1.300 
1.482 
1.703 
..067 
1.102 

20 
40 

58 
78 
10 
15 

48.67 
45.38 
39.91 
29.03 
36.78 
34.08 

15.2 
16.8 
14.8 
15.1 
15.6 
15.0 

1.173 
1.151 
1.277 
1.458 
1.609 
1.739 

25 
21 
36 
56 
70 
81 

31.82 
31.56 
30.41 
29.87 
25.17 
20.83 

(Kolb,  Bull.  Soc.  Ind.  Mullhouse,  1872.  224.) 

Coefficient  of  absorption  for  H2SO4  (1.841 
sp.  gr.  at  15°  and  760  mm.)  is  28.14  at  17°, 
and  28.86  at  16°.  (Dunn,  C.  N.  43.  121.) 


(Dunn,  C.  N.   1882,  45.  272;  Seidell,  Solu- 
bilities, 1st  Ed.) 

Coefficient  of  absorption  in  H2SO4  (sp.  gr. 
=  1.841)  =5.8;  (sp.  gr.  =  1.839)  =8.9.  (Lunge.) 


Solubility  in  salts +Aq  at  35°. 

1  =  coefficient  of  absorption  of  SO2  in  the  given  salt  solution  at  35°. 
lo  =  coefficient  of  absorption  of  SO2  in  water  at  35° =22.43. 


Salt 

3-normal 

2.5-normal 

2-normal 

1.5-normal 

1  -normal 

0.5-normal 

KI 

1 

45.43 

41.87 

38.04 

34.64 

30.25 

26.30 

l-lo 

23.00 

19.44 

15.61 

12.21 

7.82 

3.87 

KBr 

1 

36.14 

34.12 

31.93 

29.64 

27.49 

24.83 

l-lo 

13.71 

11.69 

9.50 

7.21 

5.01 

2.40 

KC1 

1 

30.02 

28.93 

27.94 

26.54 

25.15 

23.74 

l-lo 

7.59 

6.50 

5.31 

4.11 

2.72 

1.31 

KCNS 

1 

42.94 

38.13 

35.05 

32.03 

28.79 

25.63 

l-lo 

18.51 

15.70 

12.62 

9.60 

6.36 

3.20 

NH4N08 

1 

27.43 

26.66 

25.57 

24.78 

24.23 

23.35 

l-lo 

5.00 

4.23 

3.14 

2.35 

1.80 

0.92 

KN03 

1 

27.33 

26.54 

25.72 

24.79 

24.03 

23.27 

l-lo 

4.90 

4.11 

3.29 

2.36 

1.60 

0.84 

904 


SULPHUR  OXIDE 


Solubility  in  salts +Aq  at  35°. — Continued. 

1=  coefficient  of  absorption  of  SO2  in  the  given  salt  solution  at  35°. 
lo=  coefficient  of  absorption  of  SO2  in  water  at  35°=  22.43. 


Salt 

3  normal 

2.5-normal 

2  normal 

1.5-normal 

1  -normal 

0.5-normal 

K(NH4)2S04 

1 

24.60 

24.23 

23.93 

23.49 

23.14 

22.91 

l-lo 

2.17 

1.80 

1.50 

1.06 

0.71 

0.48 

^CdI2 

1 
l-lo 

24.30 

23.99 

23.71 

23.38 

23.06 

22.75 

1.87 

1.56 

1.28 

0.95 

0.63 

0.32 

^Na2S04 

1 

19.27 

19.79 

20.20 

20.81 

21.35 

21.88 

l-lo 

—3.16 

—2.64 

—2.23 

—1.62 

—1.08 

—0.55 

^CdBr2 

1 

19.17 

19.70 

20.60 

20.81 

21.46 

21.88 

l-lo 

—3.26 

—2.73 

—1.83 

—1.62 

—0.97 

—0.55 

^CdCl2 

1 

18.68 

19.23 

20.02 

20.55 

21.23 

21.73 

l-lo 

—3.75 

—3.20 

—2.41 

—1.88 

—1.20 

—0.70 

HCdS04 

1 

l-lo 

16.25 

17.41 

18.31 

19.42 

20.43 

21.45 

—6.81 

—5.02 

—4.12 

—3.01 

—2.00 

—0.98 

Solubility  in  salts  -f  Aq  at  25°. 

1  =  coefficient  of  absorption  of  SO2  in  the  given  solution  at  25°. 
lo  =  coefficient  of  absorption  of  SO2  in  water  at  25°  =  32.76. 


Salt 

3-normal 

2.5-normal 

2-normal 

1.5-normal 

1  -normal 

0.5-normal 

Kl 

1 

68.36 

62.63 

56.75 

50.58 

44.76 

38.66 

l-lo 

35.60 

29.87 

23.99 

17.82 

12.00 

5.90 

y2cdi2 

1 

35.77 

34.98 

34.74 

34.16 

33.76 

33.27 

l-lo 

3.01 

2.22 

1.98 

1.40 

1.00 

0.51 

NH4Br 

1 

52.25 

49.17 

46.06 

42.78 

39.46 

36.28 

l-lo 

19.49 

16.41 

13.30 

10.02 

6.70 

3.52 

KBr 

1 

52.26 

48.87 

44.96 

42.41 

39.11 

35.94 

l-lo 

19.00 

15.71 

12.70 

9.15 

6.35 

3.18 

NaBr 

1 

37.74 

36.84 

36.26 

35.27 

34.54 

33.76 

l-lo 

4.98 

4.08 

3.50 

2.51 

1.78 

1.00 

^CdBr2 

1 

27.46 

28.15 

29.27 

30.17 

31.01 

31.91 

l-lo 

—5.30 

—4.61 

—3.49 

—2.59 

—1.75 

—0.85 

NH4C1 

1 

42.78 

41.37 

39.76 

38.06 

36.37 

34.58 

l-lo 

10.02 

8.61 

7.00 

5.30 

3.61 

1.80 

KC1 

1 

42.27 

40.96 

39.32 

37.76 

36.05 

34.42 

l-lo 

9.51 

8.20 

6.56 

5.00 

3.29 

1.66 

SULPHUR  OXIDE 


905 


Solubility  in  salts+Aq  at  25° — -Continued. 
ption  of  s 
lo=  coefficient  of  absorption  of 


1=  coefficient  of  absorption  of  ^O2  in  the  given  solution  at  25°. 

SO2 


2  in  water  at  25°=  32.76. 


Salt 

3-normal 

2.5-normal 

2-normal 

1.5-normal 

l-normal 

0.5-normal 

NaCl 

1 

31.36 

31.51 

31.76 

31.96 

32.25 

32.46 

l-lo 

—1:40 

—1.25 

—1.00 

—0.80 

—0.51 

—0.30 

MOdCb 

1 

26.06 

27.09 

28.16 

29.46 

30.55 

31.66 

l-lo 

—6.70 

—5.67 

—4.60 

—3.30 

—2.21 

—1.10 

NH4CNS 

1 

61.46 

57.01 

52.26 

47.26 

42.74 

37.78 

l-lo 

28.70 

24.25 

19.50 

14.50 

9.98 

5.02 

KCNS 

1 

61.26 

55.87 

51.86 

47.02 

42.38 

37.57 

l-lo 

28.50 

23.11 

19.10 

14.26 

9.62 

4.81 

NaCNS 

1 

48.34 

45.86 

43.37 

40.78  , 

38.24 

35.44 

l-lo 

15.58 

13.10    ' 

10.61 

8.02 

5.48 

2.68 

NH4NO3 

1 

39.14 

38.01 

37.27 

36.28 

35.07 

33.96 

l-lo 

6.38 

5.25 

4.51 

3.52 

2.31 

1.20 

KNO3 

1 

38.52 

37.57 

36.66 

35.77 

34.79 

33.80 

l-lo 

5.76 

4.81 

3.90 

3.01 

2.03 

1.04 

H(NH4)2S04 

1 

35.96 

35.47 

34.95 

34.34 

33.82 

33.35 

l-lo 

3.20 

2.71 

2.19 

1.58 

1.06 

0.59 

K2K2S04 

1 

•  •_• 

... 

33.61 

33.20 

l-lo 

... 

... 

•,•• 

0.85 

0.48 

K2Na2S04 

1 

28.44 

28.66 

29.51 

30.45  - 

31.14 

31.96 

l-lo 

—4.32 

—4.10 

—3.25 

—2.31 

—1.62 

—0.80 

^CdS04 

1 

23.76 

25.14 

26.58 

28.24 

29.71 

31.11 

l-lo 

—9.00 

—7.62 

—6.18 

—4.52 

—3.05 

—1.85 

(Fox,  Z.  phys.  Ch.  1902,  41.  462.) 

Sol.  in  Cl2-j-Aq.    Sol.  in  Br2.    Solidification  curves  determined. 
Ch.  1913,  84.  419.) 


(Van  der  Goot,  Z.  phys. 


906 


SULPHUR  OXIDE  AMMONIA 


Solubility  of  SO2  in  alcohol.    1  vol.  alcohol  at 
t°  and  760  mm.  dissolves  V  vols.  SO2  gas 
at  0°  and  760  mm. 

Distribution  of  SO2  between  H2O  and  CHC13 
at  20°. 
Ci  =  g.  SO2  per  1.  of  H2O  solution. 
c2  =  g.  SO2  per  1.  of  CHC13  solution. 

t° 

V 

t° 

v 

t° 

V 

0 
1 
2 
3 

4 
5 
6 

7 
8 

328.62 
311.98 
295.97 
280.58 
265.81 
251.67 
238.16 
225.26 
212.98 

9 
10 
11 
12 
13 
14 
15 
16 

201:33 
190.31 
179.91 
170.13 
160:98 
152.45 
144.55 
137.27 

17 
18 
19 
20 
21 
22 
23 
24 

130.61 
124.58 
119.17 
114.48 
110.22 
106.68 
103.77 
101.47 

Ci 

C-2 

Ci/C2 

1.738 
1.753 
2.326 
2.346 
2.628 
3.039 
3.058 
3.686 
3.735 
4.226 
5.269 
5.372 
6.588 
31.92 
33.26 

1.123 
1.122 
1.704 
1.703 
1.897 
2.395 
2.385 
3.063 
3.062 
3.626 
4.798 
4.813 
6.183 
33.84 
37.25 

1.55 
1.56 
1.37 
1.38 
.38 
.27 
.28 
.20 
.22 
.17 
.10 
.12 
.07 
0.94 
0.89 

(Bunsen's  Gasometry.) 

100  pts.  absolute  methyl  alcohol  dissolve 
247  pts.  SO2  at  0°  and  760  mm.;  47  pts.  at  26° 
and  760  mm.;  100  pts.  absolute  ethyl  alcohol 
dissolve  115  pts.  SO2  at  0°  and  760  mm.;  32.3 

pts.  at  26°  and  760  mm.  (de  Bruyn,  Z.  phys. 
Ch.  10.  783.) 

Sol.  hi  ether. 

Absorbed  by  oil  of  turpentine. 

Rapidly  absorbed  by  anhydrous  aldehyde  in 
the  cold,  11  pts.  aldehyde  absorbing  19  pts. 
SO2. 

Absorption  coefficient  of  aldehyde  for  S02 
is  1.4  times  greater  than  that  of  alcohol,  and 
7  times  greater  than  that  of  H2O.  (Geuther 
and  Cartmell,  Proc.  Roy.  Soc.  10.  111.) 

1  pt.  camphor  dissolves  0.880  pt.  by  weight 
(  =  308  vols.)  S02  at  0°  and  725  mm.;  1  pt. 
glacial  HC2H3O2  dissolves  0.961  pt.  by  weight 
(=318  vols.)  SO2  at  0°  and  725  mm.;  1  pt. 
formic  acid  dissolves  0.821  pt.  by  weight 
(=351  vols.)  SO2  at  0°  and  725  mm.;l  pt. 
acetone  dissolves  2.07  pts.  by  weight  (=589 
vols.)  S02  at  0°  and  725  mm.;  1  pt.  sulphuryl 
chloride  dissolves  0.323  pt.  by  weight  ( =  187 
vols.)  SO2  at  0°  and-  725  mm.  (Schulze, 
J.  pr.  (2)  24.  168.) 


Solubility  of  SO2  in  CHC13. 
C=g.  SO2  in  1  cc.  of  the  solution. 
P  =  Pressure  in  mm.  Hg. 


t 

C 

P 

§X.io< 

2.6 
3.14 
3.17 
3.43 
3.74 

0 

it 
It 
(( 
11 

0.000701 
0.001790 
0.006982 
0.03097 
0.08217 

2.7 
5.6 
22.0 
90.2 
219.6 

25 
tt 

u 
n 

u 

0.000669 
0.001712 
0.006723 
0.02954 
0.07839 

5.7 
12.9 
48.0 
208.2 

488.8 

1.17 
1.37 
1.40 
1.47 
1.60 

(Lindner,  M.  1912,  33.  645.) 


(McCrae,  Z.  anorg.  1903,  35.  12.) 

Distribution  of  SO2  between  HCl+Aq  and 

CHC13  at  20°. 

ci=g.  SO2  per  1.  of  HCl+Aq  solution. 
c2  =  g.  SO2  per  1.  of  CHC13  solution. 
HCl  =  normality  of  HCl+Aq  used. 


HCl 

Ci 

C2 

d/C2 

f 

1.86 

1.46 

1.28 

0.05-N 

3.076 
4.277 

2.830 
4.07 

1.08 
1.04 

5.340 

5.42 

0.96 

1.25 

1.41 

0.88 

1.324 

1.416 

0.93 

0.1  -N      < 

2.78 

3.08 

0.90 

3.86 

4.08 

0.94 

5.161 

5.715 

0.90 

1.268 

1.509 

0.84 

0.2  -N      < 

1.914 
2.464 

2.274 
3.040 

0.84 
0.81 

3.967 

4.898 

0.81 

0.4  -N      | 

1.202 
1.894 

1.614 
2.263 

0.79 
0.83 

(McCrae,  Z.  anorg.  1903,  35.  14.) 

Sulphur  dioxide  ammonia,  SO2,  NH3. 

Very  hydroscopic.  Easily  sol.  in  H2O  with 
decomp.  (Schumann,  Z.  anorg.  1900,  23. 
49.) 

SO2,  2NH8.     Somewhat  hydroscopic. 

Sol.  in  H2O  with  evolution  of  NH8.  (Schu- 
mann, Z.  anorg.  1900,  23.  50.) 

5S02,  4NH3.    Very  deliquescent. 

Very  sol.  in  H2O.  (Divers  and  Ogawa, 
Chem.  Soc.  1901,  79.  1103.) 

Sulphur  in'oxide,  S08. 

.Fumes  on  air.  Miscible  with  H2O,  with 
evolution  of  much  heat.  Sol.  in  H2SO4.  De- 
comp. by  alcohol  and  ether. 


SULPHURIC  ACID 


907 


Exists  in  two  modifications,  one  of  which  is 
liquid  and  miscible  with  H2SO4,  while  the 
solid  form  is  only  slowly  sol.  therein. 
Miscible  with  CS2  at  30°,  but  at  15°  CS2 
dissolves  only  Vs  pt.  SO3,  and  SO3,  Vs  pt. 
CS2.     (Schultz-Sellack,  Pogg.  139.  480.) 
There  is  only  one  modification,  the  liquid, 
which  absorbs  H2O  and  becomes  solid.    (Rebs, 
A.  246.  356.) 
Miscible     with  liquid     SO2.       (Schultz- 
Sellack.) 
See  also  Sulphuric  acid. 

Sulphur  Aeptoxide,  S2O7. 
Fumes  on  air.    Slowly  decomp.  at  0°,  in- 
stantaneously  on   warming.     Sol.   in   cone. 
H2S04.    (Berthelot,  J.  pr.  (2)  17.  48.) 
Forms  compound  S207,  2H2O2. 
Formula  is  SO4,  according  to  Traube  (B. 
24.  1764),  and  S2O7  is  SO3+S04. 
See  also  Marshall  (Chem.  Soc.  69.  771). 
Traube  (B.  26.  148)  denies  the  existence  of 
S04. 

Sulphur  oxybromide,  SOBr2. 
See  Thionyl  bromide. 

Sulphur  oxychloride,.  SOC12. 
See  Thionyl  chloride. 
SO2C12.    See  Sulphuryl  chloride. 
S206C12.   See  Pt/roSulphuryl  chloride. 
HSO3C1.  See  Sulphuryl  hydroxyl  chloride. 
S2OC14.     Decomp.  by  H2O  and  alcohol. 
(Ogier,  C.  R.  94.  446.) 
Mixture    of    about    17SC12+2SOC1«    and 
5SO2C12.    (Knoll,  B.  1898,  31.  2183.) 

Sulphur  oxyteirachloride,  S2O3C14. 
Violently  decomp.  by  H2O,  dil.  acids,  or 
alcohol.    (Millon,  A.  ch.  (3)  29.  327.) 
Sol.  in  warm  S2C12.    (Carius,  A.  106.  295.) 
Decomp.  violently  with  CS2. 

Sulphur  oxyfluoride,  SO2F2. 
See  Sulphuryl  fluoride. 
SOF2.    See  Thionyl  fluoride. 

Sulphur  ^'phosphide,  P2S. 
See  Phosphorus  monosulphide. 

Sulphur  tetraphosphide,  P4S. 
See  Phosphorus  sem^sulphide. 

Sulphuretted  hydrogen,  H2S. 
See  Hydrogen  sulphide. 

Sulphuric  acid,  H2SO4. 
Miscible  with  H20  in  all  proportions. 

Sp.  gr.  of  H2SO+Aq. 

Baume 
degrees 

Sp.  gr. 

H2S04 

Baume 
degrees 

Sp.  gr. 

aSo, 

66 
60    . 
55 
50 
45 
40 
35 
30 
25 
20 
15 
10 
5 

1.842 
1  .  725 
1.618 
1.524 
1.466 
1  .  375 
1.315 
1.260 
1.210 
1.162 
1.114 
1.076 
1.023 

100 
84.22 
74.32 
66.45 
58.02 
50.41 
43.21 
36.52 
30.12 
24.01 
17.39 
11.73 
6.60 

6.6 
60 
55 
54 
53 
52 
51 
50 
49 
48 
47 
46 
45 

.844 
.717 
.618 
.603 
.586 
.566 
.550 
.532 
.515 
.500 
.482 
.466 
.454 

100 
82.34 
74.32 
72.70 
71.17 
69.30 
68.03 
66.45 
64.37 
62.80 
61.32 
59.85 
58.02 

(Vauquelin,  A.  ch. 
76.  260.) 

(Darcet,  A.  ch. 
(2)  1.  198.) 

Sp.  gr.  of  H2SO4+Aq. 

% 
H2S04 

Sp.  gr. 
at  15° 

Sp.  gr. 

at  25° 

H2S°04 

Sp.  gr. 
at  15° 

Sp.  gr. 
at  25° 

0 
2.5 
5 
10 
15 
20 
25 
30 
35 
40 
45 

0.9986 

1  '.  0284 
.0659 
.0998 
.1378 
.1767 
.2154 
.2562 
.2976 
.3409 

0.9955 
1.0115 
1.0272 
1  .  0604 

i.ssh 

1  '.  2078 
l!2888 

50 
55 
60 
65 
70 
75 
80 
85 
90 
95 
100 

1.3866 
1.4347 
1.4860 
.5402 
.5946 
.6534 
.7092 
.7602 
1.8050 
.8318 
.8406 

1.3780 
1.4767 
1  !  5863- 

1  '.  6996 
1  '.  7940 
1  '.  8286 

(Delezenne,  1823.) 
Sp.gr.  at  15.56°,  and  b.-pt.  of  H2SO4+Aq. 

Sp.  gr. 

1.850 
1.849 
1.848 
1.847 
1.845 
.842 
.838 
.833 
.827 
.819 
.810 
.801 
.791 
.780 

%S03 

81 
80 
79 
78 
77 
76 
75 
74 
73 
72 
71 
70 
69 
68 

B.-pt. 

Sp.  gr. 

%S03 

B.-pt. 

326° 
318 
310 
301 
293 
285 
277 
268 
260 
253 
245 
238 
230 
224 

1.769 
1.757 
1.744 
1.730 
1.715 
1.699 
1.684 
.670 
.650 
.520 
.408 
.300 
.200 
.100 

67 
66 
65 
64 
63 
62 
61 
60 
58.6 
50 
40 
30 
20 
10 

217° 
210 
205 
200 
195 
190 
186 
182 
177 
143 
127 
115 
107 
103 

(Dalton,  N.  Syst.  2.  210.) 
Sp.  gr.  of  H2S04+Aq  at  15°. 

Sp.  gr. 

&, 

H2lo4 

Sp.  gr. 

1  .  5975 
1  .  5760 
1  .  5503 
1  .  5280 
1  .  5066 
1.4860 
1.4660 
1.4460 
1.4265 
1  .  4073 
1  .  3884 
1.3697 
1  .  3530 
1  .  3345 
1.3165 

& 

H2fo4 

1.8485 
1  .  8460 
1.8410 
1.8336 
1  .  8233 
1.8115 
1  .  7962 
1  .  7774 
1  .  7570 
1  .  7360 
1.7120 
1  .  6870 
1  .  6630 
1.6415 
1  .  6204 

81.54 
79.90 
78.28 
76.65 
75.02 
73.39 
71.75 
70.12 
68.49 
66.86 
65.23 
63.60 
61.97 
60.34 
58.71 

100 
98 
96 
94 
92 
90 
88 
86 
84 
82 
80 
78 
76 
74 
72 

57.08 
55.45 
53.82 
52.18 
50.55 
48.92 
47.29 
45.66 
44.03 
42.40 
40.77 
39.14 
37.51 
35.88 
34.25 

70 
68 
66 
64 
62 
60 
58 
56 
54 
52 
50 
48 
46 
44 
42 

908 


SULPHURIC  ACID 


Sp.  gr.  of  H2S04-f-Aq  at  15°.  —  Continued. 

Correction  of  sp.  gr.  for  temperature,  to  be  added  for  a 

lowering  of  the  temp,  of  10°,  or  subtracted  for  a 

oorr 

33nondmg  increase. 

Sp.  gr. 

S04 

H2S°04 

Sp.  gr. 

SOs 

H2S04 

Sp.  gr. 

Sp.  gr. 

Sp.  gr. 

of  acid 

Corr.        of  acid 

Corr. 

of  acid 

Corr. 

.2999 

32.61 

40 

1.1410 

16.31 

20 

at  o° 

atO° 

atO° 

.  2823 
.2854 
.2190 
.  2334 

30.98 
29.35 
27.72 
23  .  09 

38 
36 
34 
32 

.  1246 
.1090 
.0953 
.0809 

14.68 
13.05 
11.41 
9.78 

18 
16 
14 
12 

1.04 
1.07 
1.10 

0.002         1.15 
0.003         1.20 
0  .  004         1  .  30 

0.005 
0.006 
0.007 

1.45 
1.70 
1.85 

0.008 
0.009 
0  .  0096 

'.  .2184 
.2032 

21.46 
22.83 

30 

28 

.0882 
1  .  0544 

8.  15 
6.52 

10 

8 

(Bineau.) 

.1876 
.1706 
1  .  1549 

21.20 
19.57 
17.94 

26 
24 
22 

1  .  0405 
1  .  0288 
1.0140 

4.89 
3.28 
1.63 

6 
•      4 
2 

Sp.  gr. 
gr. 

of  H2SO4+Aq  at  15°.    a  =  %;  b=sp. 
if  %  is  SO3;  c  =  sp.  gr.  if  %  is  H2SO4. 

a 

b 

c 

a 

b 

c 

(Ure,  Schw.  J.  35.  444.) 

1 

1. 

009 

1.0064 

51 

.530 

.408 

2 

1. 

017 

1.013 

52 

.545 

.418 

3 

1. 

025 

1.019 

53 

.556 

.428 

4 

034 

1.0256 

54 

.573 

.438 

Sp.  gr.  of  H2S04+Aq. 

5 

041 

1.032 

55 

ra 

.585 

'...448 

At  0° 

At  15° 

7 

058 

l!o464 

DO 

57 

.sis 

'  !469 

Degrees 

Sp.  gr. 

,  -  __, 

,  .  .  . 

8 

067 

1.0536 

58 

1.627 

.480 

Baume 

% 

% 

/o 

% 

9 

076 

.061 

59 

1.642 

.490 

SOs 

H2SO4 

SOs 

H2SO, 

10 

085 

.068 

60 

1  .  656 

.510 

5 

1.036 

5.1 

4.2 

5.4 

4.5^ 

11 

095 

.0756 

61 

1.675 

.512 

10 

1.075 

10.3 

8.4 

10.9 

8.9 

12 

104 

.083 

62 

1.689 

.523 

15 

20 

1.116 
1   161 

15.5 
21  2 

12.7 
17.3 

16.3 
22  4 

13.3 

18  3 

13 

114 

.091 

63 

1.701 

.534 

25 

1.209 

27.2 

22.2 

28.3 

23'l 

14 

123 

.098 

64 

1.716 

.545 

30 

.252 

33.6 

27.4 

34.8 

28.4 

15 

133 

.106 

65 

1.730 

.557 

33 
35 
38 

.296 
.320 
.332 

37.6 
40.4 
41.7 

30.7 
33.0 
34.1 

38.9 
41.6 
43.0 

31.8 
34.0 
35.1 

16 
17 

142 
150 

.1136 
.121 

66 

67 

1.742 
1.755 

.578 
.580 

37 

.345 

43.1 

35.2 

44.3 

30.2 

18 

160 

.129 

68 

1.770 

.592 

38 
39 
40 

.357 
.370 
.383 

44.5 
45.9 
47.3 

33.3 
37.5 
38.6 

45.5 
46.9 

48.4 

37.2 
38.3 
39.5 

19 
20 

170 

180 

.136 
.144 

69 
70 

1.781 
1.792 

.604 
.615 

41 

.397 

48.7 

39.7 

49.9 

40.7 

21 

190 

.1516 

71 

1.802 

.627 

42 
43 

1.410 
1  421 

50.0 
51  4 

40.8 
41  9 

51.2 
52  5 

41.8 
42  9 

22 

200 

.159 

72 

1.810 

.639 

44 

l'438 

52^8 

43^1 

54^0 

44^1 

23 

210 

1.167 

73 

1.819 

.651 

45 

1.453 

54.3 

44.3 

55.4 

45.2 

24 

220 

.174 

74 

1.825 

.663 

46 

47 

48 

1.468 
1.483 
1.498 

55.7 
57.1 

58.5 

45.5 
46.6 

47.8 

53.9 
58.2 
59.6 

46.4 
47.5 
48.7 

25 

26 

I. 

229 
239 

.182 
.190 

75  • 
76 

1.830 
1.834 

.675 
.686 

49 

1.514 

60.0 

49.0 

61.1 

50.0 

27  ' 

1. 

248 

.198 

77 

1.837 

.698 

50 
51 

1.530 
1   546 

61.4 
62  9 

50.1 
51   3 

62.6 
63.9 

51.1 
52  2 

28 

1. 

258 

1.2066 

78 

1.839 

.710 

52 

1^563 

64  A 

52^6 

65^4 

53  '4 

29 

1. 

268 

1.215 

79 

1.841 

1.722 

53 

1.580 

65.9 

53.8 

66.9 

54.6 

30 

1. 

278 

1.223 

80 

1.842 

1.734 

54 
55 
55 

1.597 
1.615 
1.634 

67.4 
68.9 
70.5 

55.0 
56.2 
57.5 

68.4 
70.0 
71.6 

55.8 
57.1 

31 
32 

1. 
1. 

288 
300 

1.231 
1.239 

81 

82 

1.745 
1.756 

57 

1.652 

72.1 

58.8 

73.2 

59.  '7 

33 

1. 

310 

1.2476 

83 

1.767 

58 
59 
60 

1.671 
1.691 
1.711 

73.6. 
75.2 
76.9 

60.1 
61.4 

62.8 

74.7 
76.3 
78.0 

61.0 
62.3    ' 
63.6 

34 
35 

1. 

1. 

320 
332 

1.256 
1.264 

84 
85 

•.  .  . 

1.777 
.786 

61 

1  .  732 

78.6 

64.2 

79.8 

65.1 

36 

344 

1.272 

86 

.794 

62 
63 
64 

1.753 
1.774 
1.798 

80.4 
82.4 
84.6 

65.7 
67.2 
69.0 

81.7 
83.9 
88.3 

66.7 
68.5 
70.4 

37 

38 

354 
367 

1.281 
1.289 

87 
88 

.802 
.809 

65 

1.819 

87.4 

71.3 

89.5 

73.0 

39 

378 

1  .  2976 

89 

.816 

66.5 
65.8 
66 

.830 
.837 
.842 

89.1 
90.4 
91.3 

72.2 
73.8 
74.5 

91.8 
94.5 
100.0 

74.9 

77. 
81.6 

40 
41 

390 
401 

1.306 
1.315 

90 
91 

.822 
.827 

63.2 

.846 

92.5 

75.5 

42 

415 

.324 

92 

.831 

66.4 
66.6 

.852 
857 

95.0 
100.0 

77.5 
81   6 

43 

1 

427 

.333 

93 

.  .  . 

1.834 

44 

1. 

440 

.342 

94 

1.8356 

(Bineau.  A.  ch.  (3)  26.  121.) 

45 
46 

1. 
1. 

451 
465 

.351 
1.361 

95 

96 

1.8376 
1.8384 

47 

1. 

478 

1.370 

97 

1.840 

48 

1. 

490 

1.379 

98 

1.8406 

The  sp.  gr.  found  at  t°  can  be  reduced  to  so.  er.  at 

49 

1. 

501 

1  .  3886 

99 

1.842 

0°  by  multiplying 

u      144-38 

using  the  follow- 

50 

1. 

517 

1.398 

100 

1.8426 

Dyi443»-t  '  or  by 

ing  table.     (Bineau.) 

(Bineau,  calculated  by  Gerlach,  Z.  anal.  8.  292.) 

SULPHURIC  ACID 


909 


Sp.  gr.  of  H2SO4+Aq  at  15°;  H2O  at  0°  =  1. 

Sp.  gr.  of  H2SO4,  etc.  —  Continued. 

Hio, 

Sp.gr. 

% 
HiS04 

Sp.  gr. 

H2S04 

Sp.  gr. 

Sp.gr 

& 

HiS°O4 

Sp.  gr. 

& 

A. 

i 

1.006 

35 

.264 

68 

.592 

1.150 

17.07 

20.91 

1.455 

45.31 

55.50 

2 

1.012 

36 

.272 

69 

.604 

.155 

17.59 

21.55 

1.460 

45.69 

55.97 

3 

1.018 

37 

.281 

70 

.615 

.160 

18.11 

22.19 

1.465 

46.07 

56.43 

4 

1.025 

38 

.290 

71 

.626 

.165 

18.64 

22.83 

1.470 

46.45 

56.90 

5 

1.032 

39 

.298 

72 

.638 

.170 

19.06 

23.47 

1.475 

46.83 

57.37 

6 

1.039 

40 

.307 

73 

.650 

.175 

19.69 

24.12 

1.480 

47.21 

57.83 

7 

1.046 

41 

.316 

74 

.662 

.180 

20.21 

24.76 

1.485 

47.57 

58.28 

8 

.053 

42 

.324 

75 

.674 

.185 

20.73 

25.40 

1.490 

47.95 

58.74 

9 

.061 

43 

.333 

76 

.684 

.190 

21.26 

26.04 

1.495 

48.34 

59.22 

10 

.069 

44 

.342 

77 

.697 

.195 

21.78 

26.68 

1.500 

48.73 

59.70 

11 

.076 

45 

1.352 

78 

.710 

.200 

22.30 

27.32 

1.505 

49.12 

60.18 

12 

.084 

46 

1.361 

79 

1.721 

.205 

22.82 

27.95 

1.510 

49.51 

60.65 

13 

.091 

47 

1.370 

80 

1.732 

.210 

23.33 

28.58 

1.515 

49.89 

61.12 

14 

.099 

48 

1.379 

81 

1.743 

.215 

23.84 

29.21 

1.520 

50.28 

61.59 

15 

.106 

49 

1.389 

82 

1.753 

.220 

24.36 

29.84 

1.525 

50.66 

62.06 

16 

.114 

50 

1.399 

83 

1.763 

.225 

24.88 

30.48 

1.530 

51.04 

62.53 

17 

.122 

51 

.409 

84 

1.773 

.230 

25.39 

31.11 

1.535 

51.43 

63.00 

18 

.129 

52 

.418 

85 

1.783 

.235 

25.88 

31.70 

1.540 

51.78 

63.43 

19 

.137 

53 

.428 

86 

1.792 

.240 

26.35 

32.28 

1.545 

52.12 

63.85 

20 

.145 

54 

.438 

87 

.800 

.245 

26.83 

32.86 

1.550 

52.46 

64.26 

21 

.153 

55 

.448 

88 

.807 

.250 

27.29 

33.40 

1.555 

52.79 

64.67 

22 

.161 

56 

.459 

89 

.814 

.255 

27.76 

34.00 

1.560 

53.12 

65.08 

23 

.168 

57 

.469 

90 

.820 

.260 

28.22 

34.57 

1.565 

53.46 

65.49 

24 

.176 

58 

.480 

91 

.825 

.265 

28.69 

35.14 

1.570 

53.80 

65.90 

25 

.184 

59 

.491 

92 

.8294 

.270 

29.15 

35.71 

1.575 

54.13 

66.30 

26 

.191 

60 

.501 

93 

.8339 

.275 

29.62 

36.29 

1.580 

54.46 

66.71 

27 

.199 

61 

.512 

94 

.8372 

.280 

30.10 

36.87 

1.585 

54.80 

67.  13 

28 

.207 

62 

.523 

95 

.8390 

.285 

30.57 

31.45 

1.590 

55.18 

67.59 

2.9 

1.215 

63 

.535 

96 

.8406 

.290 

31.04 

38.03 

1.595 

55.55 

68.05 

30 

1.223 

64 

.546 

97 

.8410 

.295 

31.52 

38.61 

1.600 

55.93 

68.51 

31 

1.231 

65 

1.558 

98 

.8412 

.300 

31.99 

39.19 

1.605 

56.30 

68.97 

32 

1.239 

66 

1.569 

99 

.8403 

.305 

32.46 

39.77 

1.610 

56.68 

69.43 

33 

1.247 

67 

1.580 

100 

.8384 

.310 

32.94 

40.35 

1.615 

57*05 

69.89 

34 

1.256 

.315 

33.41 

40.93 

1.620 

57.40 

70.32 

" 

qon 

oq    oo 

d.1   E;O 

IrJOCT 

C  T      ^7CT 

TA     *7  A 

(From  1-91  %  according  to  Kolb,  calcu- 
lated by  Gerlach;  from  92-100%  according  to 
Lunge  and  Naef,  calculated  by  Gerlach,  Z. 

.  oZU 

.325 
.330 
.335 

oo  .  oo 

34.35 
34.80 
35.27 

41  .  OvJ 

42.08 
42.66 
43.20 

.625 
1.630 
1.635 
1.640 

57.75 
58.09 
58.43 

58.74 

70.74 
71.16 
71.57 
71.99 

anal.  27.  316.) 

.340 

35.71 

43.74 

.645 

59.10 

72.40 

.345 

36.14 

44.28 

.650 

59.45 

72.88 

Sp.  gr.  of  H2SO4  at  15°  compared  with  H2O 
at  4°  and  0  mm.  pressure. 

.350 
.355 
.360 

36.58 
37.02 
37.45 

44.82 
45.35 
45.  8S 

.655 
.660 
.665 

59;  78 
60.11 
60.46 

73.23 
73.64 
74.07 

Q__        _ 

% 

% 

% 

% 

.365 

37.89 

46.41 

.670 

60.82 

74.51 

op.  gr. 

80s 

H2SO4 

Sp.  gr. 

S03 

H2S04 

1.370 

IO^Tfr 

38.32 

OO      ^7CT 

46.94 

Arj       A*? 

.675 

61.20 

74.97 

1.000 

0.07 

0.09 

1.075 

8.90 

10.90 

.375 
1.380 

o8.75 
39.18 

47.47 
48.00 

.680 
.685 

61.57 
61.93 

75.42 
75.86 

1.005 

0.68 

0.83 

1.080 

9.47 

11.60 

1.385 

39.62 

48.53 

.690 

62.29 

76.30 

1.010 

1.28 

1.57 

1.085 

10.04 

12.30 

1.390 

40.05 

49.06 

.695 

62.64 

76.73 

1.015 

1.88 

2.30 

1.090 

10.60 

12.99 

1.395 

40.48 

49.59 

.700 

63.00 

77.17 

1.020 

2.47 

3.03 

1.095 

11.16 

13.67 

1.400 

40.91 

50.11 

.705 

63.35 

77.60 

1.025 

3.07 

3.76 

1.100 

11.71 

14.35 

1.405 

41.33 

50.63 

1.710 

63.70 

78  04 

1.030 

3.67 

4.49 

1.105 

12.27 

15.07 

.410 

41.76 

51.15 

1.715 

64.07 

i  O  .  vTx 

78  48 

1.035 

4.27 

5.23 

1.110 

12.82 

15.71 

.415 

42.17 

51.66 

1.720 

64.43 

I  O  .  "O 

78  Q2 

1.040 

4.87 

5.96 

1.115 

13.36 

16.36 

.420 

42.57 

52.15 

1.725 

64.78 

t  O  .  «7^ 

7Q  3« 

1.045 

5.45 

6.67 

1.120 

13.89 

17.01 

.425 

42.96 

52.63 

1.7SO 

65  .  14 

4  <j  .  OvJ 

7Q  80 

1.050 

6.02 

7.37 

1.125 

14.42 

17.66 

.430 

43.36 

53.11 

1.735 

65.50 

/  y  .  ou 
80  94 

1.055 

6.59 

8.07 

1.130 

14.95 

18.31 

1.435 

43.75 

53.59 

1.740 

65.86 

j\j  .  ^  jt 
8O  fi8 

1.060 

7.16 

8.77 

1  .  135 

15.48 

18.96 

1.440 

44.14 

54.07 

1.745 

66.22 

3\J  .  Uo 

81    19 

1.065 

7.73 

9.47 

1.140 

16.01 

19.61 

1.445 

44.53 

54.55 

1.750 

66.58 

ox  .  J-^ 
81    ^fi 

1.070 

8.32 

10.19 

1.145 

16.54 

20.26 

1.450 

44.92 

55.03 

1.755 

66.94 

>1  .  OU 

82.00 

910 


SULPHURIC  ACID 


Sp.  gr.  of  H2SO4,  etc.  —  Continued. 

Sp.  gr.  of  cone.  H2SO4,  etc.  —  Continued. 

M 

% 

/o 

% 

%  H2S04 

Sp.  gr. 

%  H2S04 

Sp.  gr. 

Sp.  gr. 

SO  3 

TT  G(~), 

Sp.  gr. 

SOa 

H2SO.j 

95.61 

1.8414 

93.32 

1.8352 

.760 

67.30 

82.44 

1.829 

75.03 

91.90 

95.55 

1.8413 

93.29 

1.8351 

.765 

67.65 

82.88 

.830 

75.19 

92.10 

95.50 

1.8412 

93.26 

1.8350 

.770 

68.02 

83.32 

.831 

75.35 

92.30 

95.45 

1.8411 

93.23 

1.8349 

.775 

68.49 

83.90 

.832 

75.53 

92.52 

95.40 

1.8410 

93.20 

1.8348 

.780 

68.98 

84.50 

.833 

75.72 

92.75 

95.35' 

1.8409 

93.17 

1.8347 

.785 

69.74 

85.10 

.834 

75.96 

93.05 

95.30 

1.8408 

93.14 

1  .  8346 

.790 

69.96 

85.70 

.835 

76.27 

93.43 

95.25 

1.8407 

93.12 

1.8345 

.795 

70.45 

86.30 

.836 

76.57 

93.80 

95.21 

1.8406 

93.09 

1.8344 

.800 

70.94 

86.90 

.837 

76.90 

94.20 

95.16 

1.8405 

93.06 

1.8343 

.805 

71.50 

87.60 

.838 

77.23 

94.60 

95.12 

1.8404 

93.00 

1.8342 

.810 

72.08 

88.30 

.839 

77.55 

95.00 

95.08 

1.8403 

92.98 

1.8341 

.815 

72.69 

89.05 

.840 

78.04 

95.60 

95.04 

1.8402 

92.95 

1.83o9 

.820 

73.51 

90.05 

.8405 

78.33 

95.95 

95.00 

1.8101 

92.93 

1  .  8338 

.821 

73.63 

9.0.20 

.8415 

79.19 

97.00 

94.96 

1.8400 

92.90 

1.8337 

.822 

73.80 

90.40 

.8410 

79.76 

97.70 

94.92 

1.8399 

92.87 

1.8336 

.823 

73.96 

90.60 

.8415 

80.16 

98.20 

94.88 

1.8398 

92.84 

1.8335 

.824 

74.12 

90.80 

.8400 

80.57 

98.70 

94.84 

1.8397 

92.82 

1.8334 

.825 

74.29 

91.00 

.8400 

80.98 

99.20 

94.81 

1.8396 

92.79 

1.8333 

1.826 

74.49 

91.25 

.8395 

81.18 

99.45 

94.77 

1.8395 

92.77 

1.8332 

1.827 

74.69 

91.50 

.8390 

81.39' 

99.70 

94.73 

1.8394 

92.73 

1.8331 

1.828 

74.86 

91.70 

.8385 

81.59 

99.95 

94.69 

r\A   t*  rr 

1.8393 

Ioono 

92.71 

1.8330 

1O  OOA 

(Lunge  and  Isler,  Zeit.  angew.  Ch.  9.  129.) 

y4.oo 
94.61 

.8392 
1.8391 

92^66 

.  83^9 

1.8328 

94.57 

1.8390 

92.63 

1.8327 

Sp.  gr.  of  cone.  £[2804+  Aq  at  15°. 

94.53 
94.49 

1.8389 
1.8388 

92.61 
92.59 

1.8326 
1  .  8325 

%  H2SO4 

Sp.  gr. 

%  H2S04 

Sp.  gr. 

94.46 

1.8387 

92.56 

1.8324 

Q4.  40 

1   OOO£! 

QO  P\4. 

1  OQOQ 

100 

1.8384 

99.02 

1.8417 

CJT:  .  T:^J 

94.38 

1^8385 

92^52 

J.  .  oO^SO 

1.8322 

99.98 

1.8385 

98.98 

1.8418 

94.34 

1.8384 

92.49 

1.8321 

99.96 

1.8386 

98.94 

1.8419 

94.31 

1.8383 

92.46 

1  .  8320 

99.94 

1.8387 

98.84 

1.8420 

94.27 

1.8382 

92.44 

1.8319 

99.92 

•  1.8388 

98.84 

1.8421 

94.24 

1.8381 

92.41 

1.8318 

99.90 

1.8389 

98.78 

1.8422 

94.20 

1.8380 

92.39 

1.8317 

99.88 

1.8390 

98.71 

1.8423 

94.17 

1.8379 

92.37 

1.8316 

99.86 

1.8391 

98.63 

.8424 

94.13 

1.8378 

92.34 

1.8315 

99.84 

1.8392 

98.56 

.8425 

94.10 

1.8377 

92.32 

1.8314 

99.81 

1.8393 

98.48 

.8426 

94.07 

1  .  8376 

92.29 

1.8313 

99.78 

1.8394 

98.40 

.8427 

94.03 

1.8375 

92.27 

1.8312 

99.76 

1.8395 

98.32 

.8428 

94.00 

1.8374 

92.24 

1.8311 

99.73 

1.8396 

98.22 

.8429 

93.97 

1.8373 

92.22 

1.8310 

99.70 

1.8397 

98.08 

.8430 

93.93 

1.8372 

92.19 

1.8309 

99.67 

1.8398 

97.85 

.8431 

93.90 

1.8371 

92.17 

1.8308 

99.64 

1.8399 

97.50 

.8432 

93.87 

1.8370 

92.15 

1.8307 

99.61 

.8400 

97.10 

.8431 

93.83 

.8369 

92.12 

1.8306 

95.58 

.8401 

96.93 

1.8430 

93.80 

.8368 

92.10 

1.8305 

99.55 

.8402 

96.76 

1.8429 

93.77 

.8367 

92.07 

1.8304 

99.52 

.8403 

93.65 

1.8428 

93.74 

.8366 

92.05 

1  .  8303 

99.49 

.8404 

96.55 

1.8427 

93.71 

.8365 

92.02 

1.8302 

99.46 

.8405 

96.46 

.8426 

93.68 

.8364 

92.00 

.8301 

99.43 

1.8406 

96.39 

.8425 

93.65 

.8363 

91.98 

.8300 

99.40 

1.8407 

96.31 

.8424 

93.62 

.8362 

91.95 

.8299 

99.37 

1.8408 

96.24 

.8423 

93.59 

.8361 

91.93 

.8298 

99.33 

1.8409 

96.16 

.8422 

93.56 

.8360 

91.91 

1.8297 

99.29 

1.8410 

96.09 

.8421 

93.53 

.8359 

91.88 

1.8296 

99.25 

1.8411 

98.02 

.8420 

93.50 

.8358 

91.86 

1.8295 

99.22 

1.8412 

95.95 

.8419 

93.47 

1.8357 

91.84 

1.8294 

99.19 

1.8413 

95.88 

.8418 

93.44 

1.8356 

91.81 

1  .  8293 

99.16 

1.8414 

95.81 

.8417 

93.41 

1.8355 

91.78 

1  .  8292 

99.11 

1.8415 

95.74 

.8416 

93.38 

1.8354 

91.76 

1  .  8291 

99.06 

1.8416 

95.67 

.8415 

93.35 

1.8353 

91.74 

1.8290 

SULPHURIC  ACID 


911 


Sp.  gr.  of  cone.  H2SO4,  etc.  —  Continued. 


%  H2S04 

Sp.  gr. 

%  H2SO4 

Sp.  gr. 

91.72 

.8298 

90.78 

1.8244 

91.70 

.8288 

90.76 

1.8243 

91.68 

.8287 

90.74 

1.8242 

91.65 

.8286 

90.72 

1.8241 

91.63 

.8285 

90.70 

1.8240 

91.61 

.8284 

90.68 

1.8239 

91.59 

.8283 

90.66 

1.8238 

91.56 

1  .  8282 

90.64 

1.8237 

91.54 

1.8281 

90.62 

1.8236 

91.52 

1.8280 

90.60 

1.8235 

91.50 

1.8279 

90.59 

1.8234 

91.47 

1.8278 

90.57 

1.8233 

91.45 

1.8277 

90.55 

1.8232 

91.43 

1.8276 

90.53 

1.8231 

91.41 

1.8275 

90.51 

1.8230 

91.39 

1.8274 

90.49 

1.8229 

91.37 

1.8273 

90.47 

1.8228 

91.35 

1.8272 

90.46 

1.8227 

91.32 

1.8271 

90.44 

1.8226 

91.30 

1.8270 

90.42 

1.8225 

91.28 

1.8269 

90.40 

.8224 

91.26 

1.8268 

90.38 

.8223 

91.24 

1.8267 

90.37 

.8222 

91.22 

1.8266 

90.35 

.8221 

91.20 

1.8265 

90.33 

.8220 

91.18 

1  .  8264 

90.31 

.8219 

91.16 

1.8263 

90.29 

.8218 

91  .  14 

1.8262 

90.28 

.8217 

91.12 

.8261 

90.26 

.8216 

91'.  10 

.8260 

90.24 

.8215 

91.08 

.8259 

90.23 

.8214 

91.06 

.8258 

90.20 

.8213 

91-04 

.8257 

90.18 

.8212 

91.02 

.8256 

90.17 

.8211 

91.00 

.8255 

90.15 

.8210 

90.98 

.8254 

90.13 

.8209 

90.96 

.8253 

90.11 

.8208 

90.94 

1  .  8252 

90.10 

.8207 

90.92 

1.8251 

90.08 

1.8206 

90.90 

1.8250 

90.06 

1.8205 

90.88 

1.8249 

90.04 

1.8204 

90.86 

1.8248 

90.02 

1.8203 

90.84 

1.8247 

90.01 

1.8202 

90.82 

1.8246 

89.99 

1.8201 

90.80 

1.8245 

89.97 

1.8200 

(Richmond  [calculated  from  Pickering,  Chein 
Soc.  57.  64],  Jour.  Soc.  Ch.  Ind.  9.  479.) 


Sp.  gr.  of  cone.  H2SO4+Aq  at  15 


HsS04 


90 
*90.20 

91 
•91.48 

92 
*92.83 

93 

94 
*94.84 

95 
*95.97 


Sp.  gr. 

1.8185 
1.8195 
1.8241 
1.8271 
1.8294 
1.8334 
1.8339 
1.8372 
1.8387 
1.8390 
1.8406 


96 

97 
*97.70 

98 

*98.39 
*98.66 

99 

*99.47 
100 
*  100.  35 


Sp.  gr. 


1.8406 
1.8410 
1.8413 
1.8412 
1.8406 
1.8409 
1.8403 
1.8395 
1.8384 
1.8411 


*Determined  by  experiment. 
(Lunge  and  Naef,  Dingl.  248.  91.) 
Sp.  gr.  of  H2SO4+Aq  at  room  temp,  con- 
taining : 

7  .  875  15  .  503  23  .  429%  H2SO4 

1.0651  1.1305  1.2003 

(Wagner,  W.  Ann.  1883,  18.  265). 

Sp.  gr.  of  H2SO4+Aq  at  25°. 


Concentration  of  HzSCh+Aq 


1  —  normal 

V2—     " 

V4-  " 


Sp.  gr. 


1.0303 
1.0154 
1.0074 
1.0035 


(Wagner,  Z.  phys.  Ch.  1890,  5.  40.) 
Sp.  gr.  of  dil.  H2SO4+Aq. 


G.  -equivalents 
H2SO4  per  liter 

t 

Sp.  gr.  t°/t° 

0.005049 
0.01009 
0.01512 
0.02014 
0.03014 

17.343 
•     17.360 
17.382 
17.398 
17.419 

1  .  0002082 
1.0004020 
1  .  0005879 
1.000769 
1.001125 

0.002526 
0.005050 
0.01006 
0.02005 
0.03001 
0.04980 
0.09864 
0.146560 
0.19354 
0.28942 
0.47466 

18.039 
18.040 
18.040 
18.040 
18.039 
18.040 
18.048 
18.070 
18.080 
18.052 
18.055 

1.0001065 
1.0002084 
1.0004009 
1.0007668 
1.0011208 
1.0018096 
1.003460 
1.005045 
1.008580 
1.009686 
1.015616 

0.4980 
4.980 

17.73 
17.95 

1.01634 
1  .  15234 

0.005176 
0.01035 
0.01551 
0.12648 
0.25151 
0.37672 
0.50503 

12.997 
13.020 
13.005 
'      13.031 
13.011 
13.007 
12.998 

1.0002106 
1.000411 
1  .  000603 
1.004438 
1  .  008565 
1  .  012639 
1.016758 

(Kohlrausch,  W.  Ann.  1894,  53.  28.) 


912 


SULPHURIC  ACID 


Sp.gr.  of  H2SO4+Aq. 

Crf    TJ  Of\                              *?n  co             an  no             oe  TT 

Sp.  gr.  of  fuming  H2SO4  at  35°. 

70  -"-2> 

Sp.gr 

3V_/4                                 /».UO              UU.»O              OU./  / 

.  20°/20°         1.7383       1.5181       1.2719 

Total 

Free 

SO  3% 

Sp.  gr. 

Total 
SO.,  % 

Free 

Sp.  gr. 

%  Hoi 

in  in         A 

Tfi 

/O  •LJ  "k 

Sp.  gr 

.  20°/20°         1.0685       1.0317 

81.63 

0 

1.8186 

91.1* 

J        52 

1.9749 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896 

81.99 

2 

1.8270 

91.  5f 

)      54 

1.9760 

19.268.) 

82.36 

4 

1.8360 

91.91 

[      56 

1.9772 

Sp.  gr 

of  N-H2SO4+Aq  at  18°/4°  =  1.0306 

82.73 

6 

1.8425 

92.  2£ 

J      58 

1.9754 

(Loomis,  W.  Ann.  1896,  60.  550,.) 

83.09 

8 

1.8498 

92.  6£ 

i      60 

1.9738 

Sp.   gr.  of  H2SO4+Aq  at  19.4°,   when  p  = 
percent  strength  of  solution;  d  =  observec 
density;  w  =  volume  cone,  in  grams  pei 

/                             \ 

83.46 
83.82 
84.20 
84.56 

10 
12 
14 
16 

1.8565 
1.8627 
1.8692 
1.8756 

93.  OS 
93.  3£ 
93.  7£ 
94.11 

J      62 
5      64 
>      66 
68 

1.9709 
1.9672 
1.9636 
1.9600 

ft 

/  P       —       i 

84.92 

18 

1.8830 

94.  4£ 

>      70 

1.9564 

L> 

c  \Too~   / 

85.30 

20 

1.8919 

94.  8£ 

72 

1.9502 

P 

d 

w 

85.66 
86.03 

22 

24 

1  .  9020 
1.9092 

95.21 
95.55 

74 
76 

1  .  9442 
1.9379 

94.10 
84.59 
73.08 
61.35 
40.72 
31.94 
23.77 
14.72 
9.802  . 
4.826 

.8380 
.7998 
.6743 
.5341 
.3220 
.2430 
.1747 
.1023 
.0670 
.0320 

1.7295 
1  .  5223 
1.2235 
0.9412 
0.5383 
•   0.3970 
0.2792 
0.1623 
0.1046 
0.0498 

86.40 
86.76 

87.14 
87.50 
87.87 
88.24 
88.60 
88.97 
89.33 
89.70 
90.07 

26 

28 
30 
32 
34 
36 
38 
40 
42 
44 
46 

1.9158 
1  .  9220 
1  .  9280 
1.9338 
1  .  9405 
1  .  9474 
1.9534 
1.9584 
1.9612 
1  .  9643 
1  .  9672 

95.95 
96.32 
96.69 
97.05 
97.42 
97.78 
98.16 
98.53 
98.90 
99.26 
99.63 

78 
80 
82 
84 
86 
88 
90 
92 
94 
96 
98 

1.9315 
1.9251 
1.9183 
1.9115 
1.9046 
1.8980 
1.8888 
1.8800 
1.8712 
1.8605 
1.8488 

(Barnes,  J.  Phys 

.  Chem.  1898,  2.  546. 

90.44 

48 

1  .  9702 

100.00 

100 

1.8370 

Sp.  gr.  of  H2SO4+Aq  at  20°. 

90.81 

50 

1  .  9733 

Normality  of 
H2S04+Aq 

%  H2S04 

Sp.  gr. 

(Knietsch,  B.  1901,  34.  4101.) 

11 

53 

70.07 

.6129 

Sp.  gr.  of  H2SO4+Aq  at  15°/15°  in  air. 

9 

01 

59.26 

.4901 

Sp.  gr. 

%  H2SO4 

Sp.  gr 

%  H2S04 

Sp.  gr. 

%  H2S04 

6 

95 

i 

y  .  lu 

.3872 

4 

77 

36^68      . 

.2756 

1.000 

0.00 

1.028 

4.12 

1.056 

8.19 

3 

008                25.00 

.1791 

1.001 

0.15 

1.029 

4.26 

1.057 

8.33 

1 

002 

9.25 

.0612 

1.002 

0.31 

1.030 

4.41 

1.058 

8.47 

(Forchheimer,  Z.  phys.  Ch.  1900,  34.  27.) 

1.003 
1.004 

0.46 
0.60 

1.031 
1.032 

4.56 
4.70 

1  .  05£ 
1.060 

8.62 
8.76 

Sp.  gr.  of  cone,  and  fuming  H2SO4 

at  15°  and  45° 

1.005 

0.73 

.033 

4.85 

1.031 

8.90 

1.006 

0.87 

.034 

5.00 

1.052 

9.04 

H2S04 

SO3  % 

90.% 

Sp.  gr.  at-  15 

0   Sp.  gr.  at  45° 

1.007 

1.01 

.035 

5.14 

.063 

9.18 

Inno 

11  c 

fT     OQ 

95.98 

78.35 

1.8418 

.  UUo 

1.009 

.  1O 

1.30 

.'037 

5'44 

.'065 

9.'47 

96.68 

78.92 

1.8429 

1.010 

1.45 

.038 

5.58 

.066 

9.61 

96.99 

79.18 

1.8431 

1.011 

1.60 

.039 

5.73 

.087 

•9.75 

97.66 

79.72 

1  .  8434  ma? 

C.      ... 

1.012 

1.75 

.040 

5.88 

1.068 

9.89 

98.65 

80.53 

1.8403 

1.013 

1.89 

.041 

6.03 

1.069 

10.04 

99.40 

81.14 

1.8388  mir 

I.      ... 

1.014 

2.04 

.042 

6.17 

1.070 

10.18 

99.76 

81.44 

1.8418 

1.015 

2.19 

.043 

6.32 

1.071 

10.31 

100.00 

81.63 

o.'o 

1.8500 

'.822 

1.016 

2.34 

1.044 

6.46 

1.072 

10.45 

83.46 

10.0 

1.888 

.858 

1.017 

2.49 

1.045 

6.60 

1.073 

10.59 

85.30 

20.0 

1.920 

.887 

1.018 

2.64 

1.046 

6.75 

1.074 

10.73 

87.14 

30.0 

1.957 

.920 

1.019 

2.79 

1.047 

6.89 

1.075 

10.87 

88.97 

40.0 

1.979 

.945 

1.020 

2.93 

1.048 

7.04 

1.076 

11.00 

90.81 

50.0 

2.009 

.  964  max. 

1.021 

3.08 

1.049 

7.18 

1.077 

11.14 

92.65 

60.0 

2.020  max. 

1.950 

1.022 

3.23 

1.050 

7.32 

1.078 

11.28 

94.48 

70.0 

2.018 

1.942 

1.023 

3.38 

1.051 

7.47 

1.079 

11.42 

96.32 

80.0 

2.008 

1.890 

1.024 

3.53 

1.052 

7.61 

1.080 

11.56 

98.16 

90.0 

1.990 

1.864 

1.025 

3.67 

1.053 

7.76 

1.081 

11.69 

100.00 

LOO.O 

1.984 

1.814 

1.026 

3.82 

1.054 

7.90 

1.082 

11.83 

097 

3    Q7 

f\f  pr 

8.04 

1  083 

1  1    Q7 

(Knietsch,  B 

1901,  34.  4102.) 

.  \j£t  I              *->  .  t/  • 

' 

SULPHURIC  ACID 


913 


Sp.  gr.  of  H2SO4+Aq  at  15°/15°  in  air.— 
Continued. 

Sp.  gr.  of  H2SO4+Aq  at  15°/15°  in  air  — 
Continued. 

Sp.gr 

%  H2S04 

Sp.gr 

%  H2S04 

Sp.  gn 

%  H2S04 

Sp.gr 

%  H2S04 

Sp.gr 

%  H2SO4 

Sp.gr 

%  H2S04 

1.084 

12.11 

1.145 

20.25 

1.206 

27.95 

1.267 

35.33 

1.328 

42.35 

1.389 

48.92 

.085 

12.24 

1.146 

20.38 

1.207 

28.08 

1.268 

35.45 

1.329 

42.46 

1.390 

49.02 

.086 

12.38 

1.147 

20.51 

1.208 

28.20 

1.269 

35.57 

1.330 

42.57 

1.391 

49.13 

.087 

12.52 

1.148 

20.64 

1.209 

28.32 

1.270 

35.68 

.331 

42.68 

1.392 

49.23 

.088 

12.66 

1.149 

20.77 

1.210 

28.45 

1.271 

35.80 

.332 

42.79 

1.393 

49.34 

.089 

12.79 

1.150 

20.90 

1.211 

28.57 

.272 

35.92 

.333 

42.90 

1.394 

49.44 

1.090 

12.93 

1.151 

21.03 

1.212 

28.69 

.273 

36.04 

.334 

43.01 

1.395 

49.54 

1.091 

13.07 

1.152 

21.16 

1.213 

28.82 

.274 

36.15 

.335 

43.12 

1.396 

49.65 

1.092 

13.20 

1.153 

21.28 

1.214 

28.94 

.275 

36.27 

.336 

43.23 

1.397 

49.75 

1.093 

13.34 

1.154 

21.41 

1.215 

29.06 

.276 

36.39 

.337 

43.35 

1.398 

49.86 

1.094 

13.48 

1.155 

21.54 

1.216 

29.18 

.277 

36.51 

.338 

43.46 

1.399 

49.96 

1.095 

13.61 

1.156 

21.67 

1.217 

29.31 

.278 

36.62 

.339 

43.57 

1.400 

50.06 

1.096 

13.75 

1.157 

21.80 

1.218 

29.43 

1.279 

36.70 

.340 

43.68 

.401 

50.16 

1.097 

13.89 

1.158 

21.93 

1.219 

29.55 

1.280 

36.86 

.341 

43.79 

.402 

50.26 

1.098 

14.02 

1.159 

22.05 

1.220 

29.69 

1.281 

36.97 

.342 

43.90 

1.403 

50.37 

1.099 

14.16 

1.160 

22.18 

1.221 

29.80 

1.282 

37.09 

.343 

44.01 

1,404 

50.47 

1.100 

14.29 

1.161 

22.31 

1.222 

29.92 

1.283 

37.21 

.344 

44.12 

1.405 

50.57 

1.101 

14.43 

1.162 

22.44 

1.223 

30.04 

1.284 

37.32 

.345 

44.23 

1.406 

50.67 

1.102 

14.56 

1.163 

22.56 

1.224 

30.17 

1.285 

37.44 

.346 

44.34 

1.407 

50.77 

1.103 

14.70 

1.164 

22.69 

1  225 

30.29 

1.286 

37.56 

.347 

44.45 

1.408 

50.88 

1.104 

14.83 

1.165 

22.82 

l'226 

30.41 

1.287 

37.68 

.348 

44.56 

1.409 

50.98 

1.105 

14.97 

1.166 

22.94 

1.227 

30.53 

1.288 

37.79 

.349 

44.67 

1.410 

51.08 

1.106 

15.10 

.167 

23.07 

1.228 

30.65 

1.289 

37.91 

.350 

44.77 

1.411 

51.18 

1.107 

15.24 

.168 

23.20 

1.229 

30.78 

.290 

38.03 

.351 

44.88 

1.412 

51.28 

1.108 

15.37 

.169 

23.32 

1.230 

30.90 

.291 

38.14 

1.352 

44.99 

1.413 

51.38 

1.109 

15.51 

.170 

23.45 

.231 

31.02 

.292 

38.26 

1.353 

45.10 

1.414 

51.48 

1.110 

15.64 

.171 

23.57 

.232 

31.14 

1.293 

38.37 

1.354 

45.21 

1.415 

51.58 

1.111 

15.78 

.172 

23.71 

.233 

31.26 

1.294 

38.49 

1.355 

45.32 

1.416 

51.68 

1.112 

15.91 

1.173 

23.83 

.234 

31.38 

1.295 

38.60 

1.356 

45.43 

1.417 

51.78 

1.113 

16.05 

1.174 

23.96 

.235 

31.50 

1.296 

38.72 

.357 

45.53 

1.418 

51.89 

1.114 

16.18 

1.175 

24.08 

1.236 

31.62 

1.297 

38.83 

.358 

45.64 

1.419 

51.99 

1.115 

16.31 

1.176 

24.21 

1.237 

31.75 

1.298 

38.95 

.359 

45.75 

1.420 

52.09 

1.116 

16.45 

1.177 

24.34 

1.238 

31.87 

1.399 

39.06 

.360 

45.86 

1.421 

52.19 

1.117 

16.58 

1.178 

24.46 

1.239 

31.99 

1.300 

39.18 

.361 

45.97 

1.422 

52.29 

1.118 

16.71 

1.179 

24.59 

1.240 

32.11 

1.301 

39.29 

.362 

46.07 

1.423 

52.39 

1.119 

16.84 

1.180 

24.71 

1.241 

32.23 

1.302 

39.41 

.363 

46.18 

1.424 

52.49 

1.120 

16.98 

1.181 

24.84 

1.242 

32.35 

1.303 

39.52 

.364 

46.29 

1.425 

52.59 

1.121 

17.11 

1.182 

24.97 

.243 

32.47 

1.304 

39.64 

.365 

46.39 

1.426 

52.69 

1.122 

17.24 

1.183 

25.09 

.244 

32.59 

1.305 

39.75 

.366 

46.50 

1.427 

52.79 

1.123 

17.37 

1.184 

25.22 

.245 

32.71 

1.306 

39.86 

.367 

46.61 

1.428 

52.89 

1.124 

17.51 

1.185 

25.34 

.246 

32.83 

1.307 

39.98 

.368 

46.71 

1.429 

52.98 

1.125 

17.64 

1.186 

25.47 

.247 

32.95 

1.308 

40.09 

.369 

46.82 

1.430 

53.08 

1.126 

17.77 

1.187 

25.59 

.248 

33.07 

1.309 

40.20 

.370 

46.92 

1.431 

53.18 

1.127 

17.90 

1.188 

25.72 

.249 

33.19 

1.310 

40.32 

.371 

47.03 

1.432 

53.28 

.128 

18.03 

1.189 

25.84 

.250 

33.31 

1.311 

40.43 

1.372 

47.14 

1.433 

53.38 

.129 

18.16 

1.190 

25.97 

.251 

33.43 

1.312 

40.54 

.373 

47.24 

1.434 

53.48 

.130 

18.30 

1.191 

26.09 

.252 

33.55 

1.313 

40.66 

1.374 

47.35 

1.435 

53.58 

.131 

18.43 

1.192 

26.22 

.253 

33.67 

1.314 

40.77 

1.375 

47.45 

1.436 

53.68 

.132 

18.56 

1  .  193 

26.34 

1.254 

33.79 

1.315 

40.88 

1.376 

47.56 

1.437 

53.78 

.133 

18.69 

1.194 

26.47 

1.255 

33.91 

1.316 

40.99 

1.377 

47.67 

1.438 

53.88 

.134 

18.82  . 

1.195 

26.59 

1.256 

34.02 

1.317 

41.11 

1.378 

47.77 

1.439 

53  97 

.135 

18.95 

1.196 

26.71 

1.257 

34.14 

1.318 

41.22 

1.379 

47.88 

1.440 

54.07  - 

.136 

19.08 

1.197 

26.84 

1.258 

34.26 

1.319 

41.33 

1.380 

47.98 

1.441 

54.17 

.137 

19.22 

1.198 

26.96 

1  .  259 

34.38 

.320 

41.45 

1.381 

48.09 

1.442 

54.27 

1.138 

19.34 

1.199 

27.09 

1.260 

34.50 

.321 

41.56 

1.382 

48.10 

1.443 

54.36 

1.139 

19.47 

1.200 

27.21 

1.261 

34.62 

.322 

41.67 

1.383 

48.30 

1.444 

54.46 

1.140 

19.60 

1:201 

27.33 

1.262 

34.74 

.323 

41.79 

1.384 

48.40 

1.445 

54.56 

1.141 

19.73 

1.202 

27.46 

1.263 

34.86 

1.324 

41.90 

1.385 

48.$) 

1.446 

54.65 

1.142 

19.86 

1.203 

27.58 

1.264 

34.98 

1.325 

42.01 

1.386 

48.61 

1.447 

54.75 

1  .  143 

19.99 

1.204 

27.71 

1.265 

35.09 

1  .326 

42.12 

1.387 

48.71 

1.448 

54.85 

1.144 

20.12 

1.205 

27.83 

1.266 

35.21 

1.327 

42.23 

1.388 

48.82 

1.449 

54.94 

914 


SULPHURIC  ACID 


Sp.  gr.  of  H2SO4-f-Aq  at  15°/15°  in  air  — 
Continued. 

Sp.  gr.  of  H2SO4+Aq  at  15°/15°  in  air  — 
Continued. 

Sp.  gr. 

%  H2S04 

Sp.  gr. 

%  H2S04 

Sp.  gr. 

%  H2S04 

Sp.  gr. 

%  H2S04 

Sp.  gr. 

%  H2S04 

Sp.  gr. 

%  H2S04 

.450 

55.04 

1.511 

60.78 

1.572 

66.23 

1.633 

71.48 

1.694 

76.65 

1.755 

82.01 

.451 

55.14 

1.512 

60.87 

1.573 

66.31 

1.634 

71.57 

1.695 

76.74 

1.756 

82.11 

.452 

55.24 

1.513 

60.96 

1.574 

66.40 

1.635 

71.65 

1.696 

76.82 

1.757 

82.21 

.453 

55.33 

.514 

61.05 

1.575 

66.49 

1.636 

71.74 

1.697 

76.91 

1.758 

82.31 

.454 

55.43 

.515 

61.14 

1.576 

66.57 

1.637 

71.82 

1.698 

76.99 

1.759 

82.41 

.455 

55.53 

.516 

61.24 

1.577 

66.66 

1.638 

71.91 

1.699 

77.08 

1.760 

82.51 

1.456 

55.62 

.517 

61.33 

1.578 

66.75 

1.639 

71.99 

1.700 

77.17 

1.761 

82.61 

1.457 

55.72 

.518 

61.42 

1,579 

66.83 

1.640 

72.07 

1.701 

77.25 

1.762 

82.71 

1.458 

55.82 

.519 

61.51 

1.580 

66.92 

1.641 

72.16 

1.702 

77.34 

1.763 

82.80 

1.459 

55.91 

.520 

61.60 

1.581 

67.01 

1.642 

72.25 

1.703 

77.42 

.764 

82.90 

1.460 

56.01 

.521 

61.69 

1.582 

67.10 

1.643 

72.33 

1  .  704 

77.51 

.765 

83.00 

1.461 

56.11 

.522 

61.78 

1.583 

67.18 

1.644 

72.42 

1  .  705 

77.60 

.766 

83.10 

1.462 

56.20 

.523 

61.87 

1.584 

67.27 

1.645 

72.50 

1.706 

77.68 

.767 

83.20 

.463 

56.30 

1.524 

61.98 

1.585 

67.36 

1.646 

72.59 

1.707 

77.77 

.768 

83.29 

.464 

56.39 

1.525 

62.05 

1.586 

67.44 

.647 

72.67 

1.708 

77.85 

.769 

83.39 

.465 

56.49 

1.526 

62.14 

1.587 

67.53 

.648 

72.76 

1.709 

77.94 

.770 

83.49 

.466 

56.59 

1.527 

62.23 

1.588 

67.62 

.649 

72.84 

1.710 

78.0,3 

.771 

83.59 

.467 

56.68 

1.528 

62.32 

.589 

67.70 

.650 

72,93 

1.711 

78.11 

1.772 

83.69 

.468 

56.78 

1.529 

62.41 

.590 

67.79 

.651 

73,01 

1.712 

78.20 

1.773 

83.78 

1.469 

56.87 

1.530 

62.50 

.591 

67.88 

.652 

73.10 

1.713 

78.28 

1.774 

83.88 

1.470 

58.97 

1.531 

62.59 

.592 

67.97 

.653 

73.18 

1.714 

78.37 

1.775 

83.98 

1.471 

57.03 

1.532 

62.68 

1.593 

68.05 

.654 

73.27 

1.715 

78.46 

1.776 

84.08 

1.472 

57.16 

1.533 

62.77 

1.594 

68.14 

1.655 

73.35 

1.716 

78.54 

.777 

84.18 

1.473 

57.25 

1.534 

62.86 

1.595 

68.23 

1.656 

73.43 

1.717 

78.63 

.77$ 

84.29 

1.474 

57.35 

1.535 

62.95 

1.596 

68.31 

1.657 

73.52 

1.718 

78.72 

.779 

84.39 

1.475 

57.44 

1.536 

63.04 

.597 

68.40 

1.658 

73.52 

1.719 

78.80 

.780 

84.50 

1.476 

57.54 

1.537 

63.13 

.598 

68.49 

1.659 

73.69 

1.720 

78.89 

.781 

84.60 

1.477 

57.63 

.538 

63.22 

.599 

68.57 

1.660 

73.77 

1.721 

78.97 

.782 

84.71 

1.478 

57.73 

.539 

63.31 

.600 

68.66 

1.661 

73.86 

1.722 

79.06 

.783 

84.81 

1.479 

57.82 

.540 

63.40 

.601 

68.74 

1.662 

73.94 

1.723 

79.15 

.784 

84.92 

1.480 

57.92 

.541 

63.49 

.602 

68.83 

.663 

74.02 

1.724 

79.23 

.785 

85.03 

1.481 

58.01 

.542 

63.58 

.603 

68.92 

.664 

74.11 

1.725 

79.32 

.786 

85.14 

1.482 

58.10 

.543 

63.67 

.604 

69.00 

.665 

74.19 

1.726 

79.41 

.787 

85.25 

1.483 

58.20 

.544 

63.76 

.605 

69.09 

.666 

74.27 

1.727 

79.49 

.788 

85'.  36 

1.484 

58.29 

1.545 

63.85 

.606 

69.17 

.667 

74.36 

1.728 

79.58 

.789 

85.47 

1.485 

58.38 

.546 

63.94 

.607 

69.26 

.668 

74.44 

1.729 

79.67 

.790 

85.60 

1.486 

58.48 

1.547 

64.03 

.608 

69.35 

1.669 

74.53 

1.730 

79.75 

.791 

85.72 

1.487 

58.57 

1.548 

64.12 

.609 

69.43 

1.670 

74.61 

1.731 

79.84 

.792 

85.84 

1.488 

58.66 

1.549 

64.20 

.610 

69.52 

1.671 

74.69 

1.732 

79.93 

1.793 

85.96 

1.489 

58.75 

1.550 

64.29 

1.611 

69.60 

1.672 

74.78 

1.733 

80.02 

1.794 

86.GAO 

1.490 

58.85 

1.551 

64.38 

1.612 

69.69 

1.673 

74.86 

1.734 

80.11 

1.795 

86.  f 

1.491 

58.94 

1.552 

64.47 

1.613 

69.78 

1.674 

74.95 

1.735 

80.20 

1.796 

86.; 

1.492 

59.03 

1.553 

64.55 

1.614 

69.86 

.675 

75.03 

1.736 

80.29 

1.797 

86.4 

.493 

59.12 

1.554 

64.64 

1.615 

69.95 

.676 

75.12 

1.737 

80.38 

1.798 

86.5, 

.494 

59.22 

.555 

64.73 

1.616 

70.03 

.677 

75.20 

1.738 

80.47 

1.799 

86.  -71 

.495 

59.31 

.556 

64.82 

1.617 

70.12 

.678 

75.29 

1.739 

80.56 

1.800 

86.84 

.496 

59.41 

.557 

64.91 

1.618 

70.20 

.679 

75.37 

1.740 

80.65 

1.801 

86.97  J 

.497 

59.50 

.558 

65.00 

1.619 

70.29 

.680 

75.46 

1.741 

80.74 

1.802 

87.101 

.498 

59.59 

.559 

65.08 

1.620 

70.38 

.681 

75.54 

1.742 

80.84 

1.803 

87.23 

.499 

59.68 

.560 

65.17 

1.621 

70.46 

.682 

75.63 

1.743 

80.92 

1.804 

87.36 

.500 

59.78 

.561 

65.26 

1.622 

70.55 

.683 

75.71 

1.744 

81.01 

1.805 

87.50 

.501 

59.87 

.562 

65.35 

1.623 

70.63 

.684 

75.80 

1.745 

81.10 

1.806 

87.64 

.502 

59.96 

1.563 

65:44 

1.624 

70.72 

.685 

75.88 

1.746 

81.19 

1.807 

87.78 

.503 

60.05 

1.564 

65.52 

1.625 

70.80 

.686 

75.97 

1.747 

81.28 

1.808 

87.92 

1.504 

60.14 

1.565 

65.61 

1.626 

70.89 

.687 

76.05 

1.748 

81.37 

1.809 

88.06 

1,505 

60.23 

1.566 

65.70 

1.627 

70.97 

.688 

76.14 

1.749 

81.46 

1.810 

88.20 

1.506 

60.33 

1.567 

65.79 

1.628 

71.06 

1.689 

76.22 

1.750 

81.55 

1.811 

88.34 

1.507 

60.42 

1.568 

65.88 

1.629 

71.14 

1.690 

76.31 

1.751 

81.64 

1.812 

88.49 

1.508 

60.51 

1.569 

65.96 

1.630 

71.23 

1.691 

76.39 

1.752 

81.73 

1.813 

88.64 

1.509 

60.60 

1.570 

63.05 

1.631 

71.31 

1.692 

76.48 

1.753 

81.82 

1.814 

88.79 

1.510 

60.69 

1.571 

66.14 

1.632 

71.40 

1.693 

76.56 

1.754 

81.92 

1.815 

88.95 

Continued  on  page  917. 


SULPHURIC  ACID 


915 


Sp.  gr.  of  H2SO4+Aq  at  t°.    Sp.  gr.  of  H2O  at  15°  =  1. 


^4 

tE 

0° 

10° 

15° 

20° 

25° 

30° 

40° 

50° 

60° 

0 

1.00074 

1.00060 

l.OOOOQ 

0.99910 

0.99794 

0.99654 

0.99311 

0.98895 

0.98418 

] 

1.00833 

1.00773 

1.00698 

1.00594 

1.00465 

1.00312 

0.99950 

0.99522 

0.99034 

2 

1.01563 

1.01466 

1.01381 

1.01266 

1.01126 

1.00963 

1.00585 

1.00143 

0.99644 

t 
t 

1.02281 

1.02153 

1.02055 

1.01928 

1.01777 

1.01607 

1.01216 

1.00761 

1.00252 

L 

1.03001 

1.02841 

1.02728 

1.02590 

1.02428 

1.02251 

1.01848 

1.01383 

1.00865 

t 

1.03728 

1.03533 

1.03406 

1.03258 

1.03086 

1.02902 

1.02487 

1.02013 

1.01484 

( 

1.04461 

1.04232 

1.04092 

1.03934 

1.03756 

1.03565 

1.03138 

1.02653 

1.02114 

7 

1.05199 

1.04939 

1.04786 

1.04618 

1.04434 

1.04235 

1.03796 

1.03302 

1.02752 

8 

1.05942 

1.05652 

1.05486 

1.05308 

1.05116 

1.04910 

1.04458 

1.03952 

1.03393 

9 

1.06689 

1.06370 

1.03192 

1.06002 

1.05799 

1.05585 

1.05119 

1.04605 

1.04041 

10 

1.07439 

1.07093 

1.06903 

1.06702 

1.06490 

1.06267 

1.05787 

1.05264 

1.04696 

11 

1.08194 

1.07821 

1.07619 

1.07408 

1.07186 

1.06955 

1.06462 

1.05930 

1.05357 

12 

1.08954 

1.08555 

1.08342 

1.08120 

1.07890 

1.07650 

1.07145 

1.06604 

1.06027 

13 

1.09718 

1.09294 

1.09071 

1.08839 

1.08600 

1.08352 

1.07834 

1.07284 

1.06703 

14 

1.10488 

1.10040 

1.09805 

1.09564 

1.09316 

1.09061 

1.08530 

1.07971 

1.07385 

15 

1.11261 

1.10790 

1.10546 

1.10295 

1.10039 

1.09776 

1.09233 

1.08666 

1.08075 

16 

1.12040 

1.11547 

1.11292 

1.11033 

1.10768 

1.10498 

1.09944 

1.09368 

1.08772 

17 

1.12823 

1.12309 

1.12045 

1.11777 

1.11505 

1.11228 

1.10661 

1.10077 

1.09476 

18 

1.13610 

1.13076 

1.12803 

1.12526 

1.12246 

1.11963 

1.11385 

1.10792 

1.10186 

19 

1.14402 

1.13848 

1.13566 

1.13282 

1.12995 

1.12704 

1.12115 

1.11514 

1.10902 

20 

1.15199 

1.14625 

1.14335 

1.14043 

1.13748 

1.13451 

1.12851 

1.12242 

1.11625 

21 

1.15998 

1.15407 

1.15109 

1.14809 

1.14508 

1.14205 

1.13594 

1.12977 

1.12353 

22 

1.16803 

1.16194 

1.15888 

1.15581 

1.15273 

1.14964 

1.14343 

1.13718 

1.13089 

23 

1.17611 

1.16986 

1.16673 

1.16359 

1.16045 

1.15731 

1.15100 

1.14467 

1.13832 

24 

1.18424 

1.17784 

1.17464 

1.17143 

1.16823 

1.16503 

1.15862 

1.15221 

1.14579 

25 

1.19240 

1.18586 

1.18260 

1.17933 

1.17607 

1.17282 

1.16631 

1.15982 

1.15335 

26 

1.20061 

1.19393 

1.19060 

1.18728 

1.18396 

1.18066 

1.17406 

1.16749 

1.16096 

27 

1.20885 

1.20204 

1.19865 

1.19527 

1.19190 

1.18854 

1.18186 

1.17522 

1.16862 

28 

1.21710 

1.21019 

1.20675 

1.20332 

1.19990 

1.19650 

1.18973 

1.18302 

1.17635 

29 

1.22539 

1.21838 

1.21489 

1.21142 

1.20796 

1.20452 

1.19767 

1.19087 

1.18414 

30 

1.23370 

1.22661 

1.22308 

1.21957 

1.21607 

1.21259 

1.20566 

1.19879 

1.19198 

31 

1.24204 

1.23487 

1.23131 

1.22776 

1.22423 

1.22071 

1.21371 

1.20677 

1.19989 

32 

1.25038 

1.24316 

1.23957 

1.23600 

1.23244 

1.22887 

1.22179 

1.21476 

1.20779 

33 

1.25878 

1.25151 

1.24789 

1.24429 

1.24069 

1.23712 

1.22999 

1.22292 

1.21589 

34 

1.26723 

1.25990 

1.25626 

1.25263 

1.24901 

1.24540 

1.23822 

1.23109 

1.22400 

35 

1.27571 

1.26834 

1.26468 

1.26102 

1.25738 

1.25375 

1.24652 

1.23933 

1.23219 

36 

1.28424 

1.27683 

1.27314 

1.26947 

1.26580 

1.26214 

1.25487 

1.24763 

1.24045 

37 

1.29283 

1.28538 

1.28167 

1.27797 

1.27429 

1.27061 

1.26329 

1.25:01 

1.24878 

38 

1.30149 

1.29400 

1.29027 

1.28655 

1.28284 

1.27915 

1.27179 

1.26448 

1.25721 

39 

1.31022 

1.30268 

1.29894 

1.29520 

1.29148 

1,28776 

1.28038 

1,27304 

1.26575 

40 

1.31901 

1.31144 

1.30767 

1.30392 

1.30018 

1.29646 

1.28905 

1.28169 

1.27440 

41 

1.32788 

1.32027 

1.31648 

1.31271 

1.30896 

.30522 

1.29779 

1.29042 

1.28311- 

42 

1.33683 

1.32917 

1.32537 

1.32158 

1.31782 

.31407 

1.30662 

1.29924 

1.29193 

43 

1.34587 

1.33817 

1.33435 

1.33054 

1.32676 

.32300 

1.31553 

1.30813 

1.30081 

44 

1.35501 

1.34727 

1.34342 

1.33960 

1.33580 

.33202 

1.32452 

1.31710 

1.30976 

45 

1.36425 

1.35647 

1.35261 

1.34877 

1.34496 

.34116 

1.33363 

1.32618 

1.31881 

46 

1.37361 

1.36579 

1.36191 

1.35805 

1.35422 

.35040 

1.34284 

1.33365 

1.32797 

47 

1.38308 

1.37522 

1.37132 

1.36744 

1.36359 

.35975 

1.35215 

1.34464 

1.33721 

48 

1.39267 

1.38476 

1.38084 

1.37694 

1.37306 

.36921 

1.36157 

1.35401 

1.34655 

49 

1.40238 

1.39441 

1.39047 

1.38654 

1.38264 

1.37877 

1.37108 

1.36349 

1.35600 

50 

1.41219 

1.40418 

1.40021 

1.39627 

1.39235 

1.38845 

1.38073 

1.37310 

1.36556 

51 

1.42214 

1.41407 

1.41007 

1.40610 

1.40215 

1.39823 

1.39047 

1.38280 

1.37524 

52 

1.43220 

1.42408 

1.42005 

1.41605 

1.41208 

1.40814 

1.40033 

1.39262 

1.38502 

916 


SULPHURIC  ACID 


Sp.  gr.  of  H2SO4+Aq.  at  t°.   Sp.  gr.  of  H2O  at  15°  =  1  Continued 


4 

w 

0° 

10° 

15° 

20° 

25° 

30° 

40° 

50° 

60° 

53 

1.44239 

1.43420 

1.43014 

1.42611 

1.42211 

1.41814 

1.41028 

.40254 

.39490 

54 

1.45269 

1.44443 

1.44034 

1.43628 

1.43225 

1.42825 

1.42034 

.41255 

.40488 

55 

1.46311 

1.45477 

1.45065 

1.44656 

1.44250 

1.43847 

1.43051 

.42268 

.41497 

56 

1.47364 

1.46523 

1.46107 

1.45695 

1.45285 

1.44880 

1.44078 

.43290 

.42515 

57 

1.48427 

1.47578 

1.47159 

1.46743 

1.46331 

1.45922 

1.45115 

.44322 

.43542 

58 

1.49499 

1.48643 

1.48221 

1.47802 

1.47387 

1.46975 

1.46162 

.45364 

.44579 

59 

1.50583 

1.49719 

1.49292 

1.48870 

1.48452 

1.48037 

1.47218 

.46415 

.45626 

60 

.51676 

1.50804 

1.50374 

1.49949 

1.49527 

1.49109 

1.48285 

.47476 

.46683 

61 

.52778 

1.51899 

1.51465 

1.51036 

1.50611 

1.50190 

1.49360 

.48546 

.47748 

62 

.53889 

1.53002 

1.52564 

1.52132 

.51703 

1.51278 

1.50442 

.49622 

.48819 

63 

.55008 

.54113 

1.53672 

1.53236 

.52804 

1.52376 

1.51533 

.50708 

.49900 

64 

.56135 

.55233 

1.54788 

1.54348 

.53913 

1.53481 

1.52632 

.51801 

.50988 

65 

.57270 

.56360 

.55912 

1.55469 

.55030 

1.54595 

1.53740 

.52903 

.52084 

66 

.58414 

.57496 

.57044 

1.56597 

.56154 

1.55716 

1.54854 

.54011 

.53187 

67 

1.59565 

.58640 

.58184 

1.57733 

.57287 

.56846 

.55978 

.55128 

.54298 

68 

1.60724 

.59792 

.59332 

1.58878 

.58427 

.57981 

.57104 

.56246 

.55408 

69 

1.61892 

.60951 

.60488 

1.60030 

.59577 

.59129 

.58247 

.57384 

.56541 

70 

1.63068 

.62118 

.61651 

1.61189 

.60732 

.60280 

.59391 

.58521 

.57672 

71 

1.64251 

1.63293 

.62821 

1.62355 

.61894 

.61437 

.60540 

.59663 

.58806 

72 

1.65439 

1.64473 

.63997 

1.63527 

.63062 

.62601 

.61696 

.60811 

.59946 

73 

1.66633 

1.65658 

.65178 

1.64704 

.64234 

.63769 

.62855 

.61961 

.61087 

74 

1.67831 

1.66847 

1.66362 

1.65883 

1.65408 

.64939 

.64015 

.63111 

.62227 

75 

1.69030 

1.68037 

1.67547 

1.67063 

1.66584 

1.66109 

.65175 

1.64260 

.63366 

76 

.70228 

1.69225 

1.68731 

1.68242 

1.67757 

1.67278 

1.66332 

1.65405 

1.64498 

77 

.71424 

1.70411 

1.69911 

1.69416 

1.68926 

1.68439 

1.67481 

1.66540 

1.65617 

78 

.72615 

1.71589 

1.71083 

1.70582 

1.70085 

1.69591 

1.68616 

1.67658 

1.66717 

79 

.73798 

.72758 

1.72243 

1.71735 

1.71231 

1.70731 

1.69741 

1.68767 

1.67809 

80 

.74970 

.73909 

1.73386 

1.72868 

1.72356 

1.71847 

1.70842 

1.69854 

1.68881 

81 

.76120 

.75038 

1.74504 

1.73979 

1.73458 

1.72942 

1.71921 

1.70916 

1.69930 

82 

.77244 

.76140 

1.75595 

1.75057 

1.74524 

1.73998 

1.72962 

1.71945 

1.70950 

83 

.78312 

.77193 

1.76642 

1.76097 

1.75557 

1.75022 

1.73972 

1.72943 

1.71937 

84 

.79316 

.78191 

1.77636 

1.77087 

1.76543 

1.76006 

1.74943 

1.73902 

1.72883 

85 

.80250 

.79123 

1.78567 

1.78016 

1.77470 

1.76929 

1.75863 

1.74816 

1.73789 

86 

.81108 

.79982 

1.79428 

1.78878 

1.78331 

1.77789 

1.76721 

1.75674 

1.74642 

87 

.81887 

.80767 

1.80214 

1.79666 

1.79123 

1.78584 

1.77519 

1.76473 

1.75445 

88 

1.82589 

.81476 

1.80926 

1.80381 

1.79839 

1.79302 

1.78242 

.77199 

1.76176 

89 

1.83216 

.82111 

1.81564 

1.81022 

1.80484 

1.79950 

1.78895 

.77856 

1.76834 

90 

1.83771 

.82677 

1.82135 

1.81597 

1.81063 

1.80532 

.79483 

.78448 

1.77429 

91 

1.84263 

.83179 

1.82642 

1.82109 

1.81580 

1.81054 

.80013 

.78985 

1.77972 

92 

1.84691 

.83619 

1.83088 

1.82561 

1.82037 

1.81516 

.80487 

.79471 

1.78470 

93 

1.85059 

.83997 

1.83471 

1.82950 

1.82432 

1.81918 

.80902 

1.79900 

1.78914 

*94 

1.85363 

1.84311 

1.83790 

1.83275 

1.82763 

1.82255 

.81253 

1.80266 

1.79296 

95 

1.85598 

1.84555 

1.84040 

1.83526 

1.83022 

1.82520 

1.81528 

1.80553 

1.79595 

96 

1.85765 

1.84729 

1.84217 

1.83709 

1.83207 

1.82708 

1.81724 

1.80758 

1.79809 

97 

1.85854 

1.84816 

1.84305 

1.83798 

1.83297 

1.82800 

1.81822 

1.80863 

1.79924 

98 

1.85836 

1.84789 

1.84275 

1.83766 

1.83264 

1.82767 

1.81792 

1.80840 

1.79912 

99 

1.85671 

1.84612 

1.84093 

1.83581 

1.83076 

1.82578 

1.81604 

1.80658 

1.79741 

100 

(1.85330) 

(1.84255) 

(1.83729) 

(1.83213) 

(1.82705) 

(1.82205) 

(1.81231) 

(1.80288) 

(1.79381) 

Auszug  aus  Band  5  der  wissenschaftlichen  Abhandlungen  der  Normaleichungskommission 
Berlin  1904,  P.  257.    Springer's  publication. 

(Domke,  Z.  anorg.  1905,  43.  176.) 


SULPHURIC  ACID 


917 


Sp.  gr.  of  H2SO4+Aq  at  15°/15°  in  air.— 

Freezing-  and  melting-points  of  H2SO4+Aq. 

Continued  from  page  915. 

Sp.  gr.  at  15° 

F.-pt. 

M.-pt. 

Sp.  gr. 

%  H2SO, 

Sp.  gr. 

%  H2S04 

Sp.  gr. 

%H2S04 

1.671 

liq.  at  —20° 

1.816 

89.11 

1.828 

91.30 

1.840 

94.57 

1.691 
1  710 

it 

.817 
.818 

89.27 
89.44 

1.829 
1.830 

91.52 
91.74 

1.841 
1.842 

94.96 
95.40 

.727 

-7.5 

-7/5 

.819 
.820 
.821 

.822 
.823 
.824 

89.61 
89.79 
89.97 
90.15 
90.33 
90.51 

1.831 
1.832 
1.833 
1.834 
1.835 
1.836 

91.98 
92.22 
92.46 
92.71 
92.98 
93.26 

1.843 
1.844 
1.8442 
1.844 
1.843 
1.842 

96.02 
96.93 
97.50 
99.08 
99.84 
99.29 

.732 
.74.9 
.767 
.7,90 

.807 
.822 

Q/19 

.5 
-0.2 

+  1-6 
+4.5 
-9.0 

liq.  at  —20° 
« 

-8.5 
+4.5 
+6.5 
+8.0 
-6.0 

1.825 

90.70 

1.837 

93.56 

1.841 

98.61 

1.826 
1.827 

90.90 
91.10 

1.838 
1.839 

93.87 
94.20 

1.840 
18.394 

98.88 
100.00 

(Lunge,  B.  15.  2644.) 

(Lunge,  calculated  by  Marshall,  J.  Soc.  Chem. 
Ind.  1902,  21.  1509. 


(Jones  and  Pearce,  Am.  Ch.  J.  1907,  38.  733.) 


Boiling-point  of  H2SO4+Aq. 


%  H2S04 

B.-pt. 

%  H2S04 

B.-pt. 

5 

101.0° 

70 

170.0° 

10 

102.0 

72 

174.5 

15 

105.5 

74 

180.5 

20 

105.0 

76 

189.0 

25 

106.5 

78 

199.0 

30 

108.0 

80 

207.0 

35 

110.0 

82  . 

218.5 

40 

114.0 

84 

227.0 

45 

118.5 

.86 

238.5 

50 

124.0 

88 

251.5 

53 

128.5 

90 

262.5 

56 

133.0 

91 

268.0 

60 

141.5 

92 

274.5 

62.5 

147.0 

93 

281.5 

65 

153.5 

94 

288.5 

67.5 

161.0 

95 

295.0 

(Lunge,  B.  11.  370.) 


Effect  of  impurities  on  sp.  gr.  of  H2SO4+Aq. 

The  figures  show 'the  increase  in  sp.  gr.  of  H2S04  + 
Aq  caused  by  adding  0.1%  of  an  impurity  to  acid  of 
different  strengths. 


Sp.  gr. 

at  20°  of 

H2S04+Aq 

containing 

M  g.  mols.  H2SO4  per  liter. 

M. 

0.01 

0.025 

0:05 

sMp:gr- 

1.000719 
0.075 

1.001907 
0.10 

1.003551 
0.25 

Sp.  gr. 

1.005152 

1.00677 

1.01618 

M. 

0.50 

0.75 

1.0 

Sp  gr. 

1.03218 

1.04760 

1.06307 

M. 

1.5 

2.0 

Sp.  gr. 

1.09345 

1.12316 

Salt 

100  % 

98% 

94  % 

80  % 

70% 

Na2S04 
CaS04 
A12(SO4)3 
Fe2(SO4)s 
PbS04 
MgS04 
As2Os 
HSNOe 

0.0011 
0.0012 
insol. 

0.0017 
0.0011 

0.00029 

0.0010 
0.0011 
insol. 

0.0014 
0,0010 
0.0013 
0.00027 

0  .  0007 
0.0009 
insol. 
0  .  0006? 
0.0015 
0.0012 

0.0008 
0  .  0007 
0.0012? 
0.0008 
insol. 
0.0009 
0.0010 
0.00023 

0.0007 
0  .  0006 
0.0011 
0.0007 
insol. 
0.0009 

(Marshall,  J.  Soc.  Chem.  Ind.  1902,  21.  1508.) 


Sp.  gr. 


of  mixtures  of  H2SO4  (96.5%)  and 
HNO3  (94%)  at  18°/18°  in  air. 


%HN03in 
mixture 

Sp.  gr. 

%HNO3in 
mixture 

Sp.  gr. 

0.00 

.8437 

22.51 

.8215 

0.57 

1.8456 

25.56 

.8112 

1.05 

1.8476 

27.29 

.8053 

4.67 

.8586 

32.53 

.7863 

7.17 

.8618 

37.03 

.7700 

7.37 

.8620 

39.49 

.7601 

7.75 

.8619 

57.78 

.6879 

9.10 

.8605 

72.89 

.6227 

11.33 

.8557 

90.76 

.5408 

12.71 

.8520 

98.19 

.5080 

16.52 

1.8414 

100.00 

.5009 

(Marshall,  J.  Soc.  Chem.  Ind.  1902,  21.  1508.) 


Miscible  with  alcohol,  with  evolution  of 
heat  and  formation  of  ethylsulphuric  acid. 

+H2O=H4SO5,  also  called  tetrahydroxyl 
sulphuric  acid.  (Marignac,  A.  ch.  (3)  39. 
184.) 

Mpt.  8.35°.    (Pickering.) 

+2H2O=H6SO6,  also  called  perhydroxyl 
sulphuric  acid. 

Mpt.  —38.9°.  (Biron,  J.  Russ.  Phys. 
Chem.  Soc.  1899,  31.  517.) 

+3H2O.  (Pickering,  Chem.  Soc.  1890, 
57.  331.) 


918 


SULPHURIC  ACID 


+4H2O.    Mpt. -75°. 
Soc.  1890,  67.  331.) 


(Pickering,  Chem 


Sp.  gr.  and  fr.  pt.  of  hydrates  of  H2SO4. 


Hydrate 

'    % 

H.S04 

Sp.  gr.  of 
the  liquid 

Fr.-pt. 

H2SO4  (pure) 

100 

1.842 

+  10.5 

H2S04+H20 

84.48 

1.777 

+  3.5 

H2SO4+2H2O 

73.08 

1.650 

-70.0 

H2SO4+4H2O 

57.65 

1.476 

-40.0 

H2SO4+6H2O 

47.57 

1.376 

—50.0 

H2SO4+8H2O 

40.50 

1.311 

-65.0 

H2SO4  +  10H2O 

35.25 

1.268 

-88.0 

H2SO4  +  11H2O 

33.11 

1.249 

-75.0 

H2SO4  +  12H2O 

31.21 

1.233 

—55.0 

H2SO4  +  13H2O 

29.52 

1.219 

—45.0 

H2SO4  +  14H2O 

28.00 

1.207 

-40.0 

H2SO4  +  15H2O 

26.63 

1.196 

-34.0 

H2SO4  +  16H2O 

25.39 

.187 

-25.6 

H2SO4  +  18H2O 

23.22 

.170 

-19.0 

H2SO4+20H2O 

21.40 

.157 

-17.0 

H2SO4+25H2O 

17.88 

.129 

-  8.5 

H2SO4+50H2O 

9.82 

.067 

-  3.5 

H2SO4+75H2O 

6.77 

.045 

0.0 

H2SO4  +  100H2O 

5.16 

.032 

+  2.5 

H2SO4+300H2O 

1.78 

.007 

+  4.5 

H2SO4  +  1000H2O 

0.54 

.001 

+  0.5 

(Pictet,  C.  R.  1894,  119.  645.) 

Sulphuric  acid,  anhydrous,  SO3. 
See  Sulphur  dioxide. 

ZH'sulphuric  (Pt/rosulphuric)  acid,  H2S2O7. 

Very   deliquescent.      Miscible  with   H2O. 

501.  in  fuming  H2SO4.     Miscible  in  liquid 

502.  (Schultz-Sellack.) 

H2S2O7,  2H2SO4.  Fumes  on  air.  (Jacque- 
lain,  A.  ch.  (3)  30.  343.) 

TWrasulphuric  acid,  H2S4Oi3. 
Fumes  on  air.     (Weber,  Pogg.  159.  313.) 

Sulphates. 

Most  sulphates  are  easily  sol.  in  H2O; 
but  Ag2SO4,  Hg2SO4,  and  CaSO4  are  only  si. 
sol.,  while  BaSO4,  SrSO4,  and  PbS04  are 
nearly  insol.  therein.  All  sulphates  are  sol. 
in  cone.  H2SO4.  Basic  sulphates  are  insol. 
in  H2O.  Most  sulphates  are  insol.  in  alcohol. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  823.) 

Aluminum  sulphate,  basic,  2A12O3,SO3+ 
5H2O. 

Slowly  sol.  in  10  mols.  HC2H302. 
(Schlumberger,  Bull.  Soc.  1895,  (3)  13.  41.) 

+7H2O.  Easily  sol.  in  8  mols.  dil.  HC1+ 
Aq.  or  in  10  mols.  10%  acetic  acid  in  24 
hours.  (Schlumberger.) 

+10H2O.  Insol.  in  H2O;  easily  sol.  in  cold 
dil.  mineral  acids,  and  HC2H3O2+Aq.  (Crum, 
A.  89.  174.) 


Min.  Felsobanyite. 

+15H2O.     Min.  Paraluminite. 

8A12O3,  5SO3+25H2O.  Insol.  in  H20;  sol. 
in  dil.  acids.  (Lowe,  J.  pr.  79.  428.) 

5A12O3,  3S03+20H2O.  Easily  sol.  in  acids. 
(Debray,  Bull.  Soc.  (2)  7.  9.) 

3A12O3  2SO3+9H2O.  Nearly  insol.  in 
cone.  H2SO4.  (Bayer,  Dirigl.  263.  211.) 

+20H2O.    Ppt. 

4A12O3,  3SO3+36H2O.  Insol.  in  H2O. 
Easily  sol.  in  dil.  mineral  acids,  and  hot 
HC2H3O2+Aq.  (Debray,  Bull.  Soc.  (2)  7.  1.) 

A12O3,  SO3  +'6H2O  =  (A1O)2SO4  +  H2O. 
Insol.  in  H2O  or  HC2H302+Aq.  SI.  sol.  in 
hot  HC1,  easily  sol.  in  warm  KOH+Aq. 
(Bottinger,  A.  244.  225.) 

+9H2O.     (Athanasesco,  C.  R.  103.  27.) 

Min.  Aluminite. 

[Al2(pH)5]SO4-t-2H2O. 

Sol.  in  HCl-fAq.  in  the  cold  with  decomp. 
Very  unstable.  (Schlumberger,  Bull.  Soc. 
1895,  (3)  13.  60.) 

3A12O3,  4SO3+9H2O.  (Athanasesco,  C.  R. 
103.271.)' 

+30H2O.  Sol.  in  144  pts.  cold,  and  30.8 
pts.  boiling  H2O.  Easily  sol.  in  HC1,  and 
HN03+Aq.  (Rammelsberg,  Pogg.  43.  583.) 

2A12O2,  3SO3.  Decomp.  by  H20  into 
3A12O3,  SO3  and  A12(SO4)3.  (Maus.) 

A12O3,  2S03=A12O(SO4)2. 

Mm.  Alumaine. 

-f-H2O.  Sol.  in  small  quantity  of  H2O,  but 
decomp.  by  a  large  quantity  into  (A1O)2SO4 
and  A12(SO4)3.  (Maus,  Pogg.  11.  80.) 

+12H2O.  Easily  sol.  in  hot  or  cold  H2O. 
Sat.  solution  contains  45%  salt  at  15°,  which 
crystallises  unchanged  on  evaporating.  (Mar- 
guerite, C.  R.  90.  354.) 

Above  basic  compounds  are  mixtures. 
Pickering,  C.  N.  45.  121,  133,  146.) 

Aluminum  sulphate,  A12(SO4)8. 

100  pts.  H2O  dissolve  (a)  pts.  A12(S04)3, 
and  (6)  pts.  A12(SO4)3+18H2O  at: 

0°        10°       20°         30°        40°       50° 
i  31.3      33.5    36.15      40.36    45.73   52.13 

86.85   95.8    107.35    127.6    167.6   201.4 

60°         70°         80°        90°         100° 
a  59.09     66.23     73.14    80.83     98.11 
6  262.6     348.2     467.3     678.8     1132. 
(Poggiale/A.  ch.  (3)  8.  467.) 

See  also  +18H2O. 

Sp.  gr.  of  Al2(SO4)3+Aq. 


% 

A12(SO4)3 

Sp.  gr.  at 

15° 

25° 

35° 

45° 

5 
10 
15 
20 
25 

1.0569 

1.1071 
1  .  1574 
1  .  2074 
1.2572 

1.0503 
1  .  1022 
1  .  1522 
1  .  2004 
1  .  2487 

1.045 
1.096 
1.146 
1.192 
1  .  2407 

1.0356 
1.085 
1  .  1346 
1.1801 
1  .  2295 

(Reuss,  B.  17.  2888.) 

SULPHATE,  ALUMINUM  AMMONIUM 


919 


Sp.  gr.  of  Al2(SO4)3+Aq  at  15°  containing: 
10  20  30%Al2(SO4)3-fl8H2O, 

1.0535     1.1105      1.1710 

40          50%  A12(SO4)3+18H2O. 
1.2355  1.3050 

Sp.  gr.  of  sat.  solution  =  1 . 34. 
(Gerlach,  Z.  anal.  28.  493.) 

Sp.  gr.  of  Al2(SO4)3+Aq.  at  25°. 


Strength  of  Al2(SO4)3+Aq 

Sp.  gr. 

1  normal 

V.      " 

V4           " 

Vs        " 

1.0550 
1.0278 
1.0138 
1.0068 

(Wagner,  Z.  phys.  Ch.  1890,  5.  35.) 

100  pts.  of  a  mixture  of  1  vol.  H2SO4+2 
vols.  H2O  dissolve  only  6.45  pts. 
A12(SO4)3.  (Baud,  C.  R.  1903,  137.  494.) 

A12(SO4)3  is  completely  pptd.  from 
Al2(SO4)3+Aq  by  an  excess  of  glacial 
HC2H3O2.  (Persoz,  A.  ch.  (2)  63.  444.) 

Solubility  of  A12(SO4)3+(NH4)2A12(SO4)4. 
See  under  (NH4)2A12(SO4)4. 

Solubility  of  A12(SO4)3+K2A12(SO4)4.    See 


*Solution  sat.  with  respect  to  both  salts. 

(Wirth  and  Bakke,  Z.  anorg.  1914,  87.  48.) 

See  also  under 


Solubility  of  Al2(SO4)3+Li2SO4  at  30°. 

Composition  of 

Solid  phase 

Solution 

Residue 

\ 

4 

•I 

4 

25.1 
21.93 
16.10 
13.63 

13.24 
11.73 
6.75 
3.44 
0.00 

0 
5.34 
14.89 
20.76 

21.71 
22.08 
24.34 
26.12 
28.0 

63^70 
14.72 

61.24 
6.92 
3.77 

4^02 
31.17 

7.22 
33.54 
37.06 

Li2SO4,  H2O 

Li2SO4.  H2O  + 
A12(SO4)3,    18H2O 
Li2S04,  4H2O 

A12(SO4)3,  18H2O 
tt 

it 

(Schreinemakers  and  de  Waal,  Ch.  Weekbl. 
1906,  3.  539.) 

100  g.  of  sat.  solution  of  A12(SO4)3  in  glycol 
contain  14.4  g.  A12(S04)3.  (de  Coninck,  Bull. 
Ac.  Roy.  Belg.  1905.  359.) 

Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37. 4328.) 

+6H2O.  Very  slowly  sol.  in  cold,  com- 
pletely sol.  in  hot  H2O. 

+8H2O.  (Margueritte-Delarcharbonny, 
C.  R.  112.  229.) 

+10H2O.  Deliquescent,  (v.  Hauer,  W. 
A.  B.  13.  449.) 

+16H2O.  Sol.  in  cone.  H2SO4.  (Baud,  C. 
R.  1903, 137.  494.) 

+17H2O.  (Gawalowski,  C.  C.  1885. 
721.) 

+18H2O.    Permanent.    (Berzelius.) 

100  g.  of  the  aqueous  solution  contain 
27.82  g.  A12(S04)3  at  25°.    (Wirth,  Z.  anorg. 
1913,  79.  361.) 


Solubility  of  A12(SO4)3  +  18H2O  in  H2SO4+Aq 
at  25°. 


under  K2A12(SO4)4. 
Solubility  in  Fe2(SO4)3+Aq  at  25°. 

H2SO4  +Aq 
%  H2S04 

100  g.  of  the  solution 
contain 
g.  A12(SO4)3 

1  00  g.  of  the  solution  contain 

0 
5.23 
9.90 
18.70 
25.50 
40.70 
52.25 
63.70 
73.64 

27.82 
29.21 
26.21 
20.44 
15.40 
5.07 
1.216 
1.243 
2.915 

g.  A12(S04)3 

g.  Fe2(SCWi 

27.82 
26.01 
24.21 
21.64 
15.22 
*10.70\ 
10.23J 

0 
6.064 
9.819 
13.02 
23.28 
31.911 
31.90} 

(Wirth,  Z.  anorg.  1913,  79.  361.) 


Hydrous  salt  is  scarcely  sol.  in  alcohol, 
(Berzelius.) 

Min.  Alunogen. 

-f-27H20.  Efflorescent.  (Margueritte- 
Delarcharbonny,  C.  R.  99.  800.) 

Aluminum  sulphate,  acid,  A12O3,  4SO8-f 
4H2O. 

Extremely  slowly  sol.  in  cold,  more  rapidly 
in  hot  H2O.  (Baud,  C.  R.  1903,  137.  493.) 

A12O3,  6SO3+10H2O.  Sol.  in  H2O;  solu- 
tion soon  de,comp.  into  A12(SO4;8+H2SO4. 
(Silberberger,  M.  1904,  25.  221.) 

Aluminum  ammonium  sulphate  (Ammonia 
alum),  (NH4)2A12(S04)4+24H20. 

100  pts.  H2O  dissolve  2.9  pts.  anhydrous 
salt  at  0°;  207.7  pts.  anhydrous  salt  at  110.6°. 
(Mulder.) 

100  pts.  H2O  dissolve  8.74  pts.  anhydrous- 
salt  at  17.5.°  (Pohl,  W.  A.  B.  6.  597.) 


920 


SULPHATE,  ALUMINUM  AMMONIUM  CHROMIUM 


100  pts.  H2O  at  t°  dissolve  pts. 

(NH4)2A12(S04)4. 

Solubility    of    NH4    alum    in    presence    of 
(NH4)2S04  and  A12(SO4)3. 

Pts. 

Pts. 

100  g.  f&t.  solution  contains 

t° 

(NH4)2A12(SO4)4 

(NH4)2A12(SC>4)4  + 

Mixture  used 

(NH4)2SO4 

g.  Al2(SO4)s 

o 

2  10 

3  90 

10 

4.99 

9.52 

Sat.  NH4  alum 

1.42. 

3.69 

20 
30 

7.74 
10.94 

15.13 
22.01 

at  18  .  5° 
20  cc.  above  sol- 

40 
50 
60 
70 

80 

14.88 
20.09 
26.70 
35.11 
45.66 

30.92 
44.11 
66.65 
90.67 
134.47 

ution  +6  g. 
cryst.  A12(SO4)3 
20  cc.  above  sol- 
ution +4g. 

(NH4)2S04 

0.45 
20.81 

16.09 
0.29 

90 
100 

58.68 
74.53 

209.31 
357.48 

(Riidorff,  1885,  B.  18.  1160.) 

(Poggiale,  A.  ch.  (3)  8.  467.) 


According  to  Locke  (Am.  Ch.  J.  1901,  26. 
174),  Poggiale's  tables  for  NH4  and  K  alums 
are  evidently  transposed,  and  the  above  data 
are  applied  by  Poggiale  to  K  alum. 

1  I.  H2O  dissolves  91.9  g.  anhydrous,  or 
191.9  g.  hydrated  salt,  or  0.387  mols.  an- 
hydrous salt  at  25°.  (Locke,  Am.  Ch.  J. 
1901,  26.  175.) 


Solubility  in  H20  at  t°. 


G.   (NH4)2 

G.  mol. 

G.  (NH4)2 

A12(S04)4 

(NH4)2 

t° 

A12(SO4)4 

+24H2O 

A12(S04)4 

per  100  g.  H2O 

per  100 

per  100 

g.H20 

g.  H20 

0 

2.10 

3.90 

0.0044 

5 

3.50 

6.91 

0.0074 

10 

4.99 

9.52 

0.0105 

15 

6.25 

12.66 

0.0132 

20 

7.74 

15.13 

0.0163 

25 

9.19 

19.19 

0.0194 

30 

10.94 

22.01 

0.0231 

40 

14.88 

30.92 

0.0314 

50 

20.10 

44.10 

0.0424 

60 

26.70 

66.65 

0.0569 

95 

109.7 

00 

0.2312- 

(Mulder,  Poggiale,  Locke;  Marino,  Gazz. 
ch.  it.  1905,  35.  II,  351;  Berkeley,  Trans. 
Roy.  Soc.  1904,  203.  A,  214,  calc.  by  Seidell,' 
Solubilities.) 


B.-pt.  of  sat.  solution  is  110.6°. 

M.-pt.  of  (NH4)2A12(S04)4+24H20  =  92°. 
(Tilden,  Chem.  Soc.  46.  409.) ;  =95°.  (Locke, 
L  c.) 

Sp.  gr.  of  aqueous  solution  at  15°  contain 
ing: 

3%  6%  9% 

1 . 0423        1 . 0141        1 . 0282  hydrous  salt.  - 

(Gerlach,  Z.  anal.  28.  495.) 


Insol.  in  alcohol.    (Mulder.) 

Solubility  of  A1(NH4)(SO4)2+12H2O  in  a 
mixture  of  93.3  g.  H2O  and  23.33  g.  glycerine 
=  6.15  g.  (Dunlop,  Pharm.  J.  1910,  85.  6.) 

Solubility  in  93.3  g.  H2O+23.3  g.  glycerine 
+3.9  g.  phenol  =  5.59  g.  A1(NH4)(SO4)2 
+12H2O.  (Dunlop.) 

Min.  Tschermigite. 


Aluminum  ammonium  chromium   sulphate, 
A12(S04)3,       (NH4)2S04,       Cr2(S04)3  + 
48H2O. 
Sol.  in  H2O;  decomp.  by  boiling.     (Vohl, 

A.  94.  71.) 

Aluminum  caesium  sulphate.  Al2Cs2(S04)4-{- 

24H20. 

100  pts.  H2O  at  17°  dissolve  0.619  pt. 
caesium  alum.  (Redtenbacher,  J.  pr.  94. 
442.) 


Solubility  in  100  pts.  H2O  at  t°  (calculated  for 
salt  dried  at  130°). 


t° 

Pts. 
alum 

t° 

Pts. 
alum 

t° 

Pts. 
alum 

0 
10 
17 

0.19 
0.29 
0.38 

25 
35 
50 

0.49 
0.69 
1.235 

65 

80 

2.38 
5.29 

(Setterberg,  A.  211.  104.) 
Solubility  in  H2O. 


Pts. 

G.  mols. 

t° 

anhydrous  salt 

anhydrous  salt 

per  litre 

per  litre 

25 

4.7 

0.013 

30 

5.89 

0.0167 

35 

7.29 

0.0207 

40 

9.00 

0.0256 

(Locke,  Am.  Ch.  J.  1901,  26.  180.) 


SULPHATE,  ALUMINUM  MAGNESIUM 


921 


Solubility  of  Al2Cs2(SO4)4  in  H2O  at  t°. 
(G.  Al2Cs2(SO4)4+24H2O  in  100  g.  solution.) 

Aluminum  chromium  sulphate,  Al2Cr2(SO4)6. 
Insol.  in  H2O. 
Al2Cr2(SO4)6,H2S04.  Insol.  in  H2O.    (Etard 
C.  R.  86.  1400.) 

Aluminum   chromium    potassium    sulphate, 

A12(SO4)3,  Cr2(SO4)3,  2K2SO4+48H2O. 
Sol.  in  H2O,  but  decomp.  on  boiling.  (Vohl.) 

Aluminum  copper  sulphate,  2A12O3,   9CuO, 
3SO3+21H2O. 
Min.  Cyanotrichite.    (Percy,  Phil.  Mag.  (3) 
36.   103.) 

t° 

%  salt 

t° 

%  salt 

0 
15 
30 
45 
60 

0.21 
0.35 
0.60 
1.04 
1.96 

75 
80 
90 
100.4 

4.12 
5.21 
9.50 
18.60 

(Berkeley,  Trans.  Roy.  Soc.   1904,  203.  A, 
214.) 

Solubility  in  100  g.  H2O  at  t°. 


o 

0 

o 

o 

t° 

•  03, 

t 

•  oo 

I 

t° 

•  CO 

t° 

0 

0.19 

26 

0.50 

52 

1.45 

78 

5.15 

1 

0.20 

27 

0.51 

53 

.51 

79 

5.40 

2 

0.21 

28 

0.52 

54 

.58 

80 

5.78 

3 

0.22 

29 

0.55 

55 

.65 

81 

6.05 

4 

0.23 

30 

0.57 

56 

1.71 

82 

6.4 

5 

0.24 

31 

0.59 

57 

1.77 

83 

6.7 

6 

0.25 

32 

0.60 

58 

1.86 

84 

7.0 

7 

0.26 

33 

0.62 

59 

1.92 

85 

7.4 

8 

0.27 

34 

0.65 

60 

2.06 

86 

7.7 

9 

0.28 

35 

0.69 

61 

2.14 

87 

8.0 

10 

0.29 

36 

0.72 

62 

2.25 

88 

8.3 

11 

0.30 

37 

0.75 

63 

2.37 

89 

8.6 

12 

0.31 

38 

0.77 

64 

2.50 

90 

8.8 

13 

0.32 

39 

0.80 

65 

2.65 

91 

9.0 

14 

0.34 

40 

0.85 

66 

2.78 

92 

9.2 

15 

0.35 

41 

0.87 

67 

2.96 

93 

9.5 

16 

0.36 

42 

0.91 

68 

3.13 

94 

9.9 

17 

0.38 

43 

0.96 

69 

3.34 

95 

10.1 

18 

0.39 

44 

1.01 

70 

3.50 

96 

10.4 

19 

0.40 

45 

1.06 

71 

3.67 

97 

10.8 

20 

0.41 

46 

1.10 

72 

3.85 

98 

11.1 

21 

0.42 

47 

1.17 

73 

4.07 

99 

11.5 

22 

0.43 

48 

1.21 

74 

4.30 

100 

12.0 

23 

0.45 

49 

1.27 

75 

4.50 

24 

0.47 

50 

1.30 

76 

4.72 

25 

0.49 

51 

1.39 

77 

4.95 

Values  from  0-7°  obtained  by  interpolation 
using  Setterberg's  values  for  0°(A.  1882,  211. 
100). 

From  80-100°    they   were    calculated  by 

extrapolation. 

(Hart  and  Huselton,  J.  Am.  Chem.  Soc.  1914, 

36.  2084.) 

Melts  in  crystal  H2O  at  106°  (Tilden, 
Chem.  Soc.  45.  409);  at  120.5°  (Erdmann)- 
at  122°  (Locke.) 


calcium   sulphate,   basic,   A1203, 
6CaO,  3SO3+32H20. 
Min.  Ettringite.      Mostly  sol.  in  H2O;  sol. 
inHCl+Aq. 


Aluminum  hydroxylamine  sulphate, 

A12(SO4)3,  (NH2OH)2SO4+24H2O. 
Sol.  in  H20.     (Meyeringh,  B.  10.  1946.) 

Aluminum  iron  (ferrous)  sulphate,  A12(SO4)8, 
FeSO4+24H2O. 

Sol.inH2O.    (Klauer,  A.  14.  261.) 

Min.  Halotrichite. 

A12(SO4)3,  2FeSO4+27H2O.  Sol.  in  H2O. 
(Berthier.) 

A12O3,  2SO3,  6FeSO4.  Easily  sol.  in  H2O. 
(Phillips.) 

A12(SO4)3  2FeS04,  H2SO4.  Insol.  in  H2O. 
(Etard,  C.  R.  87.  602.) 

Aluminum  iron  (ferric)  sulphate,  A12(SO4)3, 

Fe2(S04)3. 
Insol.  in  H20.     (Etard,  C.  R.  86.  1399.) 

A12(SO4)3,  Fe2(SO4)3,  H2SO4.  As  above 
(Etard.) 

See  Al2(SO4)3+Fe2(SO4)3,  under  A12(S04)3 
and  Fe2(SO4)3. 

Aluminum     ferrous     potassium      sulphate, 

A12(SO4)3,  12FeSO4,  2K2SO4+24H2O. 
Permanent.    SI.  sol.  in  H20.    (Dufrenoy.) 

Aluminum    lead    sulphate,    Al2Pb2(SO4)6+ 
20H2O. 

Permanent;  insol.  in  F2O.  (G.  H.  Bailey 
J.  Chem.  Soc.  Ind.  6.  415.) 

Aluminum  lithium  sulphate,  Li2Al2(SO4)4-4- 
24H2O. 

Sol.  in  24  pts.  cold,  and  0.87  pt.  hot  H2O. 
(Kralovansky,  Schw.  J.  54.  349.) 

Does  not  exist.  (Rammelsberg,  J.  B.  1847- 
48.  394;  Arfvedson;  Gmelin.) 

Aluminum  lithium  potassium   sulphate   (?). 
Sol.  in  H2O,  from  which  it  crystallises  on 
cooling.    (Joss,  J.  pr.  1.  142.) 

Aluminum    magnesium    sulphate,    MgS04) 

A12(SO4)3+22H2O. 

Min.  Pickerinqite. 

2MgSO4,  A12(SO4)3+22H2O.  Min.  Pio 
raluminite. 

3MgSO4,  A12(S04)3+36H2O.  Very  sol.  in 
H2O.  (Klauer,  A.  14.  264.) 


922 


SULPHATE,  ALUMINUM  MAGNESIUM  MANGANOUS 


Aluminum  magnesium  manganous  sulphate 
A12(SO4)3,  MgSO4,  MnSO4+25H20. 

As  sol.  in  H2O  as  K  alum.  (Kane.)  Ver} 
sol.  in  H2O.  (Smith,  Sill.  Am.  J.  (2)  18.  379. 

Min.  Bosjemanite. 

Aluminum  manganous   sulphate,   A12(SO4)3 

MnSO4+25H2O. 
Sol.  in  H20.     (Berzelius.) 
+24H2O.     Min.  Apjohnite. 

Aluminum    manganic    sulphate.    2A12(SO4)3 

Mn2(S04)3. 
Insol.  in  H20.     (Etard,  C.  R.  86.  1399.; 

Aluminum  nickel  sulphate,  A12(S04)3,  2NiSO4 

H2S04. 

Insol.  in  H2O,  but  gradually  decbmp 
thereby.  (Etard,  C.  R.  87.  602.) 

Aluminum    potassium    sulphate,    basic. 
3(A1203,    SO,),    K2S04+6H20=K2S04, 
3A12(S04,)(OH)4. 

Min.  Alunite.  Insol.  in  H2O.  Insol.  in 
cone.  HCl+Aq. 

Sol.  in  boiling  H2S04  of  1.845  sp.  gr.,  but 
more  easily  in  a  mixture  of  12  g.  H2SO4  and 
1.5  g.  H2O,  and  also  in  weaker  acids,  if  heated 
to  210°.  (Mitscherlich,  J.  pr.  81.  108.) 

+9H2O.  Min.  Lowigite.  SI.  sol.  in  boil- 
ing HCl+Aq.  (Mitscherlich,  J.  pr.  83.  455.) 

Nearly  insol.  in  HC1  or  cone.  HNO3+Aq, 
but  sol.  in  a  mixture  of  1  pt.  H2SO4  and  1  pt. 
H2O.  (Debray,  Bull.  Soc.  (2)  7.  9.) 

A12O(SO4)2,  K2SO4.  Sol.  in  H2O,  but  de- 
comp.  by  heating. 

With  varying  composition.  Precipitates. 
Insol.  in  H2O.  Very  si.  sol.  in  cold,  gradually 
in  hot  acids.  (Bley,  J.  pr.  39.  17.)  Very 
difficultly  sol.  in  warm  cone.  HCl+Aq,  but 
easily  sol.  in  KOH+Aq.  (Naumann,  B.  8. 
1630.) 


Temp. 

Pts. 

K2Al2(S04)4 

Temp. 

Pts. 

K2A1.2(S04)4 

0 

3.0 

60 

25 

5 

3.5 

70 

40 

10 

4.0 

80 

71 

15 

5.0 

90 

109 

20 

5.9 

92.5 

119.5 

30 

7.9 

100 

154 

40 

11.7 

110 

200 

50 

17.0 

111.9 

210.6 

100  pts.  H2O  dissolve  (a)  pts.  anhydrous 
alum,  and  (&)  pts.  crystallised  at  t°. 

0°  10°  20°  30°  40°  50° 
a  2.62  4.50  6.57  9.05  12.35  15.9 
65.22  9.16  13.66  19.29  27.3  36.5 

60°         '70°          80°        90°         100° 
a  21.1     26.95      35.2      50.3       70.83 
6  51.3     71.97     103.1     187.8     421.9 
(Poggiale,  A.  ch.  (3)  8.  467.) 

According  to  Locke  (Am.  Ch.  J.  1901,  26. 
174),  Ppggiale's  tables  for  NH4  and  K  alums 
are  evidently  transposed,  and  the  above 
date  are  applied  by  Poggiale  to  NH4  alum. 

100  pts.  H2O  dissolve  K2A12';S04)4+24H2O 
corresponding  to  pts.  anhydrous 
K2A12(SO4)4. 


(Mulder,  Scheik.  Verhandel.  1864.  90.) 

100  pts.  H2O  at  17°  dissolve  13.5  pts. 
K2A12(SO4)4+24H2O,  or  7.36  pts.  K2A12(SO4)4. 
Redtenbacher,  J.  pr.  94.  442.) 

Forms  supersaturated  solutions  very  easily. 
Supersat.  solutions  are  brought  to  crystallisa- 
tion by  addition  of  a  crystal  of  alum  or  an 
somorphous  substance,  as  chrome  or  iron 
alum.  Other  substances  as  NaCl,  etc.  have 
no  action.  (Thomson,  Chem.  Soc.  35.  199.) 

1  1.  H2O  dissolves  72.3  g.  anhydrous,  or 


Aluminum  potassium  sulphate  (Potash  alum), 

KA1(SO4)2+12H2O  or  K2A12(SO4)4  = 
K2SO4,  A12(SO4)3+24H2O. 

138.4  g.  hydrated  salt,  or  0.28  g.  mol.  of 
anhydrous  salt   at   25.°     (Locke,   Am.  Ch. 
J.  1901,  26.  175.) 

Sol.  in  H2O  with  absorption  of 

heat. 

Solubility  in  H2O  at  t°. 

When  100  pts.  H2O  at  10.8°  are  mixed  with 

•J    A          _~J.-.              -I,  J-T  J  -—          1  J           -t       A      O 

(g.  alum  in  1000  g.  H2O.) 

14   pts.    all 

iin,    T/ue    w 

jiup.    is    10 

kvereu    i.«. 

(Rudorff,  B.  2.  68.) 

t° 

g.  alum 

t° 

g.  alum 

Burnt  alum  is  very  slowly  sol.  in  H2O. 

0 

57.0 

75 

1280.9 

100  pts.  H2O  at  t°  dissolve  P  pts.  K2Al2(S'04)4+24H2O. 

5 

76.3 

76 

1412.1 

t° 

P 

t° 

P 

10 

84.9 

77 

1517.9 

15 

103  6 

78 

1680  1 

12.5 

7.6 

50.0 

46.7 

20 

120.3 

79 

1775.2 

21.25 
25  0 

10.4 
22  0 

62.5 
75.0 

230.0 
920.0 

25 

131.3 

80 

1950.0 

37^5 

44^1 

87  '.5 

1566'  6 

30 

184.9 

82 

2273.5 

36 

204.3 

84 

2661.5 

(Brandas,  1822.) 

40 

250.0 

Orr 

84.6 

2816.0 

Sol.  in  18  pts.  cold,  and 

1.6  pts.  boiling  H2O  (Four- 

45 

290.2 

85.1  ' 

3166.6 

croy);   in   14.12  pts.   cold,   and   0.75   pt.   boiling   H2O 
(Bergmann);  in  15  pts.  cold,  and  0.75  pt.  boiling  H2O 
(Dumas);  in  11.7  pts.  H2O  at  18.75°  (Abl). 

50 
55 

367.8 
457.7 

85.3 
85.6 

3337.2 
3372.2 

100  pts.  H..O  dissolve  14.79  pts.  alum  at  15.56°,  and 

60 

585.4 

86 

3997.8 

133.33  pts.  at  100°.     (Ure's  Diet.) 
K2Al2(SO4)4+Aq  sat.  at  15°  contains  10.939  pts.  alum 
in  every  100  pts.  H2O.     (Michel  and  Krafft.) 

65 
70 

708.4 
943.8 

87 
88 

4825.4 
6639.6 

K2Al2(SO4)  4  ~|~AQ    S8.t.   in  cold  contains    o»^yo   slum 
(Fourcroy),  6.7%  (Boerhave). 

(Marino,  Gazz.  ch.  it.  1905,  35.  (2)  351.) 

SULPHATE,  ALUMINUM  POTASSIUM 


923 


Solubility  in  H2O  at  t°. 

B.-pt.    of   K2Al2(SO4)4+Aq    containing   pts. 

K2AVSO4)4  to  100 

pts.  H2O. 

t° 

(S04)4  per 
100  g.  H20 

g.  K2Ah 
per  100  g.  H2O 

g.  mol. 
K2A12(S04)4 
perlOOg.H20 

B.-pt. 

Pts. 

K2A12(S04)4 

B.-pt. 

Pts. 
K2A12(S04)4 

o 

3  0 

5   65 

0  0058 

100.5° 

17.0 

104 

.0° 

83.9 

5 

3  5 

6  62 

0  0088 

101.0 

30.2 

104 

.5 

90.7 

10 

4  0 

7  60 

0  0077 

101.5 

41.8 

105 

.0 

97.6 

15 

5  0 

9  59 

0  0097 

102.0 

51.6 

105 

.5 

103.9 

20 

5  9 

11  40 

0  0114 

102.5 

60.4 

106 

.0 

110.5 

25 

7  23 

14  14 

0  0140 

103.0 

68.7 

106 

.5 

116.9 

30 

8.39 

16.58 

0.0162 

103.5 

76.7 

106 

.7 

120.55 

40 
50 

11.70- 
17.00 

23.83 
36.40 

0  .  0227 
0.0329 

(Gerlach,  Z.  anal.  26.  435.) 

60 
70 
80 
90 

24.75 
40.00 
71.0 
109.0 

57.35 
110.5 
321.3 
2,275.0 

0.0479 
0.0774 
0.01374 
0.2110 

K2A12(S04>4+A12(S04)3. 
K2A12(SO4)4  is  nearly  insol.  in  sat.  A12(SO4)8 
+Aq.    (Crum,  A.  89.  156.) 

92  5 

119  0 

oo 

0  2318 

Solubility  in  AVSOi)34-Aq 

Solid   Pha,sp  = 

(Mulder,  Poggiale,  Locke;  Marino,  Gazz. 

K  alum-fAl2'SO4)3. 

ch.  it.  1905,  35.  (2)  351;  and  Berkeley,  Proc. 
Roy.  Soc.  1904,  203.  A,  214,  calc.  by  Seidell, 

t° 

g'  in  lOOoV.  H2O  2 

g.  K2S04  in 
1000  g.  H2O 

Solubilities,  1st  Ed.) 

0 

234.73 

23.45 

20 

824.25 

30.85 

35 

911.02 

35.29 

M.-pt.      of      K2A12(SO4)4+24H2O=84.5° 
(Tilden,  Chem.  Soc.  45.  409.);  =92.5°  (Erd- 
mann);  =91°(Locke). 

50 
65 

77 

1,243.21 
1,598.00 
1,872.11 

59.55 
119.43 
183.80 

1.045  (Anthon);  at  15°  =  1.0488  (Michel  and 
Krafft);  at  15°  =  1.0456  (Stolba). 

Sp.  gr.  of  K2Al2(SO4)4+Aq  at  15°  con- 
taming  5%  K2A12(SO4)4  =  1.0477.  (Kohl- 
rausch,  W.  Ann.  1879.  1.) 


gr.  of  K2Al2'SO4)4+Aq  at  15°. 
K2AVSO4)4+24H2O   in    100 


pts. 

pts.  solu- 
tion; b=pts.  K2AVSO4)4  in  100  pts. 
solution;  c  =  pts.  K2AVSO4)4  for  100  pts. 
H20. 


a 

.   b 

c 

Sp.  gr. 

4 
8 
12 
13 

2.1792 
4.3584 
6.5376 
7.083 

2.2277 
4.5570 
6.9950 

7.622 

1.0210 
1.0420 
1.0641 
1.0690 

(Gerlach,  Z.  anal.  27.  280.) 


Saturated  solution  boils  at  111.9°,  and 
contains  210.6  pts.  K2A12(SO4)4+24H2O  to 
lOOpts.  H2O.  (Mulder.) 

100  pts.  H2O  contain  52  pts.  K2A12(S04)4, 
and  boils  at  104.5°.  (Griffiths.)  Crust  forms 
at  106.3°,  when  the  solution  contains  114.2 
pts.  K2A12(SO4)4  to  100  pts.  H2O.  (Gerlach, 
Z.  anal.  26.  426.) 


(Marino,  Gazz.  ch.  it.  1905,  35.  (2)  351.) 

Solubility  is  decreased  by  presence  of  Na 
alum.  (Venable,  C.  N.  1879,  40.  198.) 

Nearly  completed  pptd.  from  sat.  aq. 
solution  by  addition  or  Fc  or  Cr  alum.  (v. 
Hauer,  J.  B.  1866.  59.) 

K2Al2(S04)4+MgS04. 

K2AVSO4)4+Aq  sat.  at  10°,  and  then  sat. 
with  MgSO4  at  9°,  contains  for  100  pts. 
H20— 


Alum  (anhydrous)      . 
MgSO4       .... 

At  10° 

At  9° 

4.0 

2.7 
31.2 
33.9 

31  .'l 

(Mulder.) 

K2Al2(S04)4+k2S04. 

K2Al2(SO4)4+Aq  at  10°,  and  then  sat.  with 
K2SO4  at  same  temp.,  contains  for  100 
pts.  H2O— 


Alum  (anhydrous) 
K2S04        .      .      . 

At  10° 

At  9° 

4.0 

0.86 
9.16 

9'7 

10.20 

(Mulder.) 


924 


SULPHATE,  ALUMINUM  RUBIDIUM 


Solubility    in    K2SO4+Aq.      Solid    phase  = 
K  alum+K2SO4. 

Aluminum  rubidium  sulphate.  Al2Rb2(S04)4 
+24H20. 
100  pts.  H2O  dissolve  2.27  pts.   at  17°; 
very  sol.  in  hot  H2O.     (Redtenbacher,   J. 
pr.  94.  442.) 

Solubility  in  100  pts.  H2O  at  t°  (calculated 
for  salt  dried  at  130°). 

t° 

A12(SO4)3 
+18H2O 
in  1000  g. 
H2O 

g.  K2S04 
in  1000 
g.  H2O 

t° 

A12(SO4)3 
+18H2O 
in  1000 
g.  H20 

g.  K2S04 
in  1000 
g.  H20 

0. 
0.5 
5. 
10 
15 
30 

5.06 

8.658 
16.07 
18.52 
20.56 
39.60 

75.83 
75.18 
85.78 
96.50 
109.30 
147.80 

40 
50 
60 
70 
80 

73.88 
126.00 
249.70 
529.01 
1,044.04 

163.10 
195.40 
238.80 
323.74 
517.27 

t° 

Pts. 
alum 

t° 

Pts. 

alum 

t° 

Pts. 
alum 

0 
10 
17 

0.71 
1.09 
1.42 

25 

35 
50 

1.85, 
2.67 
4.98 

65 

80 

9.63 
21.60 

(Marino,  I.  c.) 

K2Al2(S04)4+Na2S04. 

K8Al2(SO4)4+Aq  sat.  at  10°,  and  then  sat. 
with  Na2SO    at  9°,  contains  for  100  pts. 


±12U  — 

t° 

Pts.  per  litre 

G.  mo  Is. 
anhydrous  salt 
per  litre 

Alum  (anhydrous) 
Na2SO4      .... 

At  10° 

At  9° 

4.0 

4.1 

8.8 

SA 

25 
30 

35 
40 

18.1 
21.9 

26.6 
32.2 

0.059 
0.072 
0.087 
0.106 

12.9 

Solubility    of   K2A12(S04)4+T12A12(S04)4   in 
H2O  at  25°. 


G. 

K2A12(S04)4 
per  1. 

G. 

T12A12(S04)4 
per  1. 

Solid  phase 
Mol.  % 
K2A12(S04)4 

Sp.  gr. 

69.90 

0.00 

100 

1.0591 

74.56 

0.48 

99.61 

1.0601 

67.90 

1.72 

98.48 

1.0598 

65.30 

4.52 

95.45 

1.0603 

64.95 

9.60 

91.73 

1.0605 

53.23 

18.44 

82.54 

1.0609 

45.32 

24.60 

75.12 

1.0609 

38.02 

32.48 

65.73 

1.0611 

34.54 

35.59 

61.36 

1.0611 

28.35 

42.99 

51.93 

1.0623 

10.94 

66.12 

21.34 

1.0654 

0.00 

75.46 

0.00 

1  .  0674 

(Foch,  Z.  Kryst.  Min.  1897,  28.  397.) 


Insol.  in  alcohol  of  0.905  sp.  gr.  or  less 
(Anthon,  J.  pr.  14.  125.) 

Insol.  in  acetone.  (Naumann,  B.  1904 
37.  4328.) 

Insol.  in  methyl  acetate.  (Naumann,  B 
1909,  42.  3790.) 

Solubility  in  H2O  is  increased  by  glycerine 
(Dunlop,  Pharm.  J,  1910,  31.  6.) 

Min.  Kalinite. 

+8H2O.    Stable  in  dry  air.    (Marino,  I.  c.] 

+ 14H2O.  Converted  into  ord.  alum  in 
air.  (Marino.) 


(Setterberg,  A.  211.  104) 
Solubility  in  H2O. 


(Locke,  Am.  Ch.  J.  1901,  26.  180. 

Melts  in  crystal  H2O  at  99°  (Tilden, 
Chem.  Soc.  45.  409);  at  105°  (Erdmann); 
at  109°  (Locke.) 

Aluminum    silver    sulphate,    Al2Ag2(SO4)4+ 

24H2O. 

Decomp.  by  H2O.  (Church  and  North- 
cote,  C.  N.  9.  155.) 

Aluminum  sodium  sulphate,  Al2Na2(SO4)4-f 

24H2O. 
Very  si.  efflorescent. 

Sol.  in  2.14  pts.  H2O  at  13°,  or  100  pts.  H2O  dissolve 
46.7  pts.  soda  alum.  Sol.  in  1  pt.  boiling  H2O.  (Zellner, 
Schw.  J.  36.  183.) 

100  pts.  H2O  dissolve  110  pts.  at  15.5°,  and  form  a 
liguid  of  1.296  sp.  gr.  (Ure.) 

100  pts.  H2O  dissolve  51  pts.  soda  alum  at 
16°.  (Aug6,  C.  R.  110.  1139.) 

100  pts.  H2O  dissolve  110  pts.  soda  alum 
at  0°.  (Tilden,  Chem.  Soc.  45.  409.) 

100  g.  H2O  dissolve  at: 
10°     15°     20°    25°  30° 
36 . 7  38 . 7  40 . 9  43 . 145 . 8  g.  anhydrous  salt. 
(Smith,  J.  Am.  Chem.  Soc.  1909,  31.  247.) 

M.-pt.    of    Na2Al2(SO4)4+24H2O  =  61°. 
(Tilden,  Chem.  Soc.  45.  409.);  =63.°    (Locke, 
Am.  Ch.  J.  1901,  26.  183.) 

Insol.  in  absolute  alcohol.     (Zellner.) 

Min.  Mendozite. 


SULPHATE,  AMMONIUM 


925 


Aluminum  thallous  sulphate,  T1A1(SO4)2. 

0.177  g.  mols.  of  anyhydrous  salt  are  sol. 
in  1  1.  H2O  at  25°;  or  1  1.  H2O  dissolves  75  g. 
of  the  anhydrous,  or  117.8  g.  of  the  hydrated 
salt  at  25°.  (Locke,  Am.  Ch.  J.  1901,  26. 
175.) 

Solubility  in  H2O  at  t°. 


t° 

G.  A12T12(S04)4 
in  100  g.  H2O 

G.A12T12(S04)4 
+24H20 
in  100  g.  H2O 

0 

3.15 

4.84 

5 

3.80 

5.86 

10 

4.60 

7.12 

20 

6.40 

10.00 

25 

7.60 

11.95 

30 

9.38 

14.89 

40 

14.40 

23.57 

50 

22.50 

38.41 

60 

35.36 

65.19 

(Seidell,  Solubilities,  1st  Ed.,  p.  15.) 


3A12(SO4)S,  T12SO4+96H2O.    Sol.  in  H2O. 
(Lamy.) 


Aluminum  zinc  sulphate,  A12(SO4)3,  ZnSO4  + 

24H20. 
Sol.  inH2O.    (Kane.) 


Aluminum  sulphate  chromium  chloride, 

Al(OH2)6(SO4)2CrCl2(OH2)4+2H2O. 
(Werner,  B.  1906,  39.  337.) 


Aluminum  sulphate  sodium  fluoride. 

Decomp.  by  H2O.     (Weber,   Dingl. 
112.) 


263. 


Ammonium  sulphate,  (NH4)2SO4. 

Sol.  in  H2O  with  absorption  of  heat. 

75  pts.  (NH4)2SO4  mixed  with  100  pts. 
H2O  lower  the  temperature  from  13.2°  to 
6.8°,  that  is,  6.4.°  (Riidorff,  B.  2.  68.) 

Sol.  in  1.31  pts.  H2O  at  19°.     (Schiff,  A  109.  326.) 

Sol.  in  2  pts.  H2O  at  18.75°.     (Abl.) 

Sol.  in  2  pts.  H2O  at  15.6°,  and  in  1  pt.  boiling  H2O. 
(Fourcroy.) 

100  pts.  H2O  at  62.6°  dissolve  78  pts.  (NH4)2SO4. 
(Wenzel.) 

100  pts.  H2O  at  15°  dissolve  66.739  pts.  (NH4)2SO4. 
(Michel  and  Krafft.) 

Sol.  in  1.3  pts.  cold  H2O.  (Vogel,  N.  Rep. 
Pharm.  10.  9.) 

Sol.  in  1.37  pts.  cold  H2O  at  10°.  (Mulder, 
J.  B.  1866.  67.) 

Sol.  in  1.34  pts.  H20  at  16-17°.  (v.  Hauer, 
W.  A.  B.  53,  2.  221.) 


100  pts.  H2O  dissolve  at: 

0°  10°  20°  30° 

71.00  73.65  76.30  78.95  pts.  (NH4)2SO4, 

40°  50°  6'0°  70° 

81.60  84.25  86.90  89.55  pts.  (NH4)2SO4, 

r>/-vO  f\nO  -I          O 


80° 
92.20 


90C 
94.85 


97. 50  pts.  (NH4)2SO4. 


^-ttjmaru,  \*>.  .EX.  u«7.  uuu.,; 

Solubility  in  100  pts.  H2O  at  t°. 

t° 

J 

t° 

jj 

6 

t° 

4 

z 

5 

6 

0 

70.6 

37 

80.1 

74 

93.1 

1 

70.9 

38 

80.4 

75 

93.4 

2 

71.1 

39 

80.7 

76 

93.8 

3 

71.4 

40 

81.0 

77 

94.2 

4 

71.6 

41 

81.3 

78 

94.5 

5 

71.8 

42 

81.7 

79 

94.9 

6 

72.1 

43 

82.0 

80 

95.3 

7 

72.3 

44 

82.3 

81 

96.6 

8 

72.5 

45 

82.7 

82 

96.0 

9 

72.8 

46 

83.0 

83 

96.4 

10 

73.0 

47 

83.3 

84 

96.8 

11 

73.2 

48 

83.7 

85 

97.2 

12 

73.5 

49 

84.0 

86 

97.6 

13 

73.7 

50 

84.4 

87 

98.0 

14 

74.0 

51 

84.7 

88 

98.4 

15 

74.2 

52 

85.1 

89 

98.8 

16 

74.4 

53 

85.5 

90 

99.2 

17 

74.7 

54 

85.8 

91 

99.6 

18 

74.9 

55  , 

86.2 

92 

100.0 

19 

75.1 

56 

86.6 

93 

100.4 

20 

75.4 

57 

86.9 

94 

100.8 

21 

75.7 

58 

87.3 

95 

101.2 

22 

75.9 

59 

87.7 

96 

101.6 

23 

76.2 

60 

88.0 

97 

102.1 

24 

76.4 

61 

88.4 

98 

102.5 

25 

76.7 

62 

88.7 

99 

102.9 

26 

76.9 

63 

89.1 

100 

103.3 

27 

77.2 

64 

89.5 

101 

103.8 

28 

77.5 

65 

89.9 

102 

104.2 

29 

77.8 

66 

90.2 

103 

104.6 

30 

78.0 

67 

90.6 

104 

105.1 

31 

78.3 

68 

90.9 

105 

105.5 

32 

78.6 

69 

91.3 

106 

106.0 

33 

78.9 

70 

91.6 

107 

106.5 

34 

79.2 

71 

92.0 

108 

107.0 

35 

79.5 

72 

92.4 

108.9 

107.5 

36 

79.8 

73 

92.7 

... 

... 

(Mulder,  calculated  from  his  own  and  other 
observations,  Scheik.  Verhandel.  1864.  60.) 

100  g.  (NH4)2SQ4+Aq  contain  41.4  g. 
(NH4)2SO4  at  0°.  (de  Waal,  Dissert.  1910); 
44.27  g.  at  30°.  (Schreinemakers,  Z.  phys. 
Ch.  71.  110);  47.81  g.  at  70°.  (de  Waal.) 

(NH4)2SO4+Aq  sat.  at  15°  has  sp.  gr.  1.248. 
(Michel  and  Krafft,  A.  ch.  (3)  41.  471.) 


926 


SULPHATE,  AMMONIUM 


Sp.  gr.  of  (NH4)2SO4+Aq  at  15°. 

Sp.  gr.  of  (NH4)2S04+Aq. 

%  (NH«)2S04  1 

Sp.   gr. 

o 

s 

W 

Sp.  gr. 

1 
g 

Sp.  gr. 

H(NH4)2f 
in  1000  g 

3O4  g.  mol. 
of  solution 

Sp.  gr.  16°/16° 

0 
0. 

1. 

2. 
4. 
10. 
20. 
40. 
56. 

5514 
1251 
3114 
5840 
0893 
0138 
5236 
8536 

1.000000 
1.000347 
1.000704 
1.001436 
1.002823 
1.006093 
1.012023 
1.024117 
1.033690 

1 

2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 

.0057 
.0115 
.0172 
.0230 
.0287 
.0345 
.0403 
.0460 
.0518 
.0575 
.0632 
.0690 
1.0747 
1.0805 
1.0862 
1.0920 
1.0977 

18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
34 

1.1035 
1.1092 
1.1149 
1.1207 
1.1265 
1.1323 
1.1381 
1.1439 
1  .  1496 
1  .  1554 
1.1612 
1.1670 
.1724 
.1780 
.1836 
.1892 
.1948 

35 
36 
37 
38 
39 
40 
41 
42 
43 
44 
45 
46 
47 
48 
49 
50 

1.2004 
1.2060 
.2116 
.2172 
.2228 
.2284 
.2343 
.2402 
1.2462 
1.2522 
1.2583 
1.2644 
1.2705 
1.2766 
1.2828 
1.2890 

(Dijken,  Z.  phys.  Ch.  1897,  24.  107.) 
Sp.  gr.  of  (NH4)2SO4+Aq  at  20°. 

Normality 

of 

hAq 

%  (NH4)2S04 

Sp.  gr. 

3.75 
2.964 
1.978 
0.876 
0.492 

40.28 
32.99 
23.01 
10.88 
6.275 

1 
1 
1 
1 
1 

.2289 
.1858 
.1319 
.0626 
.0352 

(Schiff,  calculated  by  Gerlach,  Z.  anal.  8.  280.) 
Sp.  gr.  of  (NH4)2SO4+Aq  at  15°. 

(Forchheimer,  Z.  phys.  Ch.   1900, 
Sp.  gr.  of  (NH4)2SO4+Aq  at 

34.  22.) 
20°. 

Solution 

Sp 

gr. 

weight  of  10  ccm. 
of  the  solution 

(NH4)2SO4 

1 

Sp.  gr. 

W 

Sp.  gr. 

H 

fc 

Sp.  gr. 

sat. 

1/4  ;; 

v!  « 

Vs     " 

1.24& 
1.196 
1.139 
1.077 
1.039 

12.  5062  g. 
11.9034" 
11.3377  " 
10.7232  " 

53.2 
39.9 
26.6 
13.3 
6.65 

(Wiener,  Z.  phys.  Chem.  1911,  71.  120.) 

B.-pt.  of  sat.  solution:  crust  formed  at 
106.2°,      solution      containing      88.2      pts. 
(NH4)2SO4  to  100  pts.  H20;  highest  temp, 
observed,  108.2°.    (Gerlach,  Z.  anal.  26.  426.) 

5 
10 

1.0292 
1.0581 

20 
30 

1.1160 
1.1730 

31 

1  .  1787 

(Kohlrausch,  W.  Ann.  1879.  1.) 

Sp.  gr.  of  (NH4)2SO4+Aq  at  15°. 


B.-pt.    of    (NH4)2SO4+Aq    containing    pts. 
(NH4)2SO4  to  100  pts.  H2O. 


%  (NH4)2S04 

Sp.  gr. 

W 

Sp.  gr. 

1 

Sp.  gr. 

3 
6 

1.0181 
1.0359 

10 
20 

1.0600 
1.1190 

30 
40 

1.1773 
1.2352 

(Gerlach,  Z.  anal.  28.  493.) 


Sp.   gr.    of    sat.    solution  =  1.248.      (Ger- 
lach.) 


B.-pt. 

Pts. 

(NH4)2SO4 

B.  pt. 

Pts. 
(NH4)2SO4 

100.5° 
101.0 
101.5 
102.0 
102.5 
103.0 
103.5 
104.0 
104.5 

7.8 
15.4 
22.8 
30.1 
37.2 
44.2 
51.1 
58.0 
64.9 

105.0° 
105.5 
106.0 
106.5 
107.0 
107.5 
108.0 
108.2 

71.8 
78.7 
85.5 
92.3 
99.1 
105.9 
112.6 
115.3 

(Gerlach,  Z.  anal.  26.  431.) 
Sol.  with  decomp.  in  HCl+Aq. 

SULPHATE,  AMMONIUM 


927 


Solubility  in  H2SO4+Aq  at  25°. 


100  g.  of  the  solution 
contain 


Mol. 

H2S04 

0.00 
0.24 
0.47 
0.97 
1.19 


1.43 

1.72 

2.20 

.60 

.71 

,82 

.96 

.20 


3.32 

3.47 
3.54 
3.76 
4.22 
5.09 


Mol. 

(NH4)2SC>4 


2.28 
3.25 
3.19 
3.15 
3.15 


3.22 
3.18 
3.02 
2.97 
3.00 
3.03 
3.10 
3.19 
3.25 


3.32 
3.20 
2.84 
2.26 
1.44 


Solid  phase 


(NH4)2S04 


(NH4)3H(S04)5 


(NH4)HSO< 


(D'Ans,  Z.  anorg.  1909,  65.  229.) 
Solubility  in  H2SO4+Aq  at  30°. 


Composition  of  the  solution 


by  wt. 
H2S04 

10.63 
10.70 
13.18 

16.67 
25.82 
27.33 
32.32 
33.12 
33.84 
33.96 
38.51 
42.12 
45.80 
45.77 
56.55 
62.43 
62.46 
63.12 
62.57 
62.83 
62.56 
62.67 
62.59 
61.63 
62.23 


by  wt. 

(NH4)2SO 

43.59 
43.25 
44.10 

42.06 
41.15 
41.16 
44.63 
45.50 
45.52 
45.31 
35.37 
30.10 
24.88 
24.30 
16.98 
20.41 
24.40 
24.20 
27.67 
29.75 
30.26 
31.86 
33.70 
36.75 
36.95 


u 

by  wt. 
H2O 

45.79 
46.05 
42.72 

41.27 

33.03 

31.51 

22.26 

21.83 

20.64 

20.73 

26.12 

27.78 

29.32 

29.93 

26.37 

17.16 

13.14 

12.68 

9.76 

8.42 

7.28 

5.47 

3.71 

1.72 

0.82 


Solid  ph£ 


(NH4)2S04 

(NH4)2S04  + 

3(NH4)2S04,  H28O. 
3(NH4)2S04,  H2S04 


(NH4)HS04 


Solubility  of  (NH4)2SO4  in  H2SO4+Aq  at  25°. 


(Van  Dorp,  Z.  phys.  Ch.  1910,  73.  285.) 


In  1000  g.  of  the 
solution 

Solid  phase 

Mol. 
SOs 

Mol. 

(NH4)2S04 

4.29 

2.17 

4.57 

1.83 

(NH4)HS04 

4.85 

1.60 

5.25 

1.36 

5.66 

1.22 

6.16 

1.26 

6.47 

1.55 

(NH4)HS04 

6.51 

1.95 

6.50 

2.37 

6.43 

2.50 

(NH4)HS04+(NH4)H3(S04)8 

7.28 

1.64 

7.99 

1.38 

(NH4)H3(S04)2 

(7.60) 

(1.74) 

(8.00) 

(1.42) 

9.02 

0.96 

9.21 

0.832 

(NH4)HS2O7 

9.60 

0.977 

9.68 

1.00 

9.67 

1.26 

(NH4)HS207+? 

10.43 

0.894 

(D'Ans,  Z.  anorg.  1913,  80.  241.) 

Very  easily  sol.,  even  in  cone.  NH4OH-f- 
Aq.    (Girard,  Bull.  Soc.  (2)  43.  522.) 

Solubility  of  (NH4)2SO4inNH4OH+Aqat250. 


In  1000  g.of  the  solution 


Mol.  (NH4)2S04 


3.28 
2.60 
2.13 
1.59 
1.16 
0.78 
0 


Mol.  (NH3)2 


0 

1.02 
1.95 
3.44 
5.35 
7.13 
9.47 


(D'Ans  and  Schreiner,  Z.  anorg.  1910,  67. 438.) 

100  pts.  H2O  dissolve  46.5  pts.  (NH4)2SO4 
and  26.8  pts.  NH4C1  at  21.5°. 

Solubility  of  (NH4)2SO4  in  NH4Cl+Aq  at  30°. 

Solid  phase 


% 
NtuCl 


0 

6.86 
14.62 
17.60 
17.93 
19.07 
19.97 
22.3 
24.06 
29.5 


(NH4)2SO4 


44 

36.15 
28.6 
25.69 
25.81 
23.22 
21.3 
16.33 
12.72 
0 


(NH4)2S04 
a 

(i 

(NH4)2SO4+NH4C1 
it 

NH4C1 


Schreinemakers,  Arch.  Neer.  Sc.  1910,  (2)  16. 

92.) 
See  also  under  NH4C1. 


928 


SULPHATE,  AMMONIUM 


(NH4)2S04+CuS04. 

Solubility  of  (NH4)2SO4+CuSO4  in  H2O  at 
16°. 


Solution 


Both  salts  in  excess 

15  cc.  sat.  sol. +3  g.  (NH4)2SO4 

15  cc.  sat.  sol. +3  g.  CuSO,5H2O 


8.55 

1.77 

15.85 


7.12 

18.16 
5.65 


(Riidorff,  B.  6.  482.) 

Solubility  of  (NH4)2SO4+CuSO4  in  H2O  at 
30°. 


0 

2.45 

5.79 

6.98 

8.19 

9.33 

17.53 

29.27 

38.32 

43.29 

44 


20.32 
20.19 
20.53 

16.77 

13.65 

11.03 

4.05 

1.57 

0.77 

0.49 

0 


Solid  phase 


CuSO4.5H2O 

CuS04,  5H20+CuS04,  (NH4)2SO4 
6H20 
CuS04,  (NH4)2S04.6H20 


CuSO4)  (NH4)2S04.6H20  + 

(NH4)2SO4 

(NH4)2SO4 


(Schreinemakers,  Arch.  Ne'er.  Sc.   1910,  15. 

12.) 
See  also  under  CuSO4. 

(NH4)2S04+FeS04. 

Solubility  of   (NH4)2SO4+FeSO4   in   H2O  + 
Aq  at  30°. 


Composition  of  the 
solution 


% 
F 


by  wt. 
eSO4 


24.90 
25.24 
25.22 

25.26 

23.59 

17.64 

13.13 

7.95 

5.70 

1.72 

0.79 

0.79 
0 


by  wt. 


0 
5.24 

5  .  93 

5.89 

6  .  44 

8.90 
11.45 
16.29 
19.64 
34.24 

43  .  86 

43.90 

44.27 


Solid  phase 


FeSO4,  7H20 

FeSO4,  7H2O  + 

FeSO4,  (NH4)2SO4>  6II2O 

FeS04,  (NH4)  2SO4,  6H2O 


FeSO4,  (NH4)  2SO4,  6H2O  + 
(NH4)2S04 


(Schreinemakers,  Z.  phys.  Ch.  1910,  71.  111.) 


(NH4)2S04+Li2S04. 

Solubility  of  (NH4)2SO4+Li2SO4. 


Temp.  =30°. 


NH4)2SO4 


44.1 

40.8 

39.5 

30 

21.6 

15 

12.5 

8.9 

0 


Li2SO4 


0 

3 

6.6 
10 
15 
20 
21.9 
23 
25.1 


Solid  phase 


(NH4)2S04 
(i 

(NH4)2SO4+NH4LiSO4 
NH4LiS04 


NH4LiSO4+Li2SO4,  H2O 
Li2SO4,  H2O 


Temp.  =50°. 


45.7 

1 

(NH4)2S04 

43.05 

5.86 

(NH4)2SO4+NH4LiSO4 

19.65 

16.35 

NH4LiSO4 

13.90 

21.20. 

tt 

13.97 

21.23 

NH4LiSO4+Li2SO4,  H2O 

11.45 

21.75 

Li2S04,  H2O 

9.63 

22.79 

tt 

8.58 

23.09 

tf 

7.56 

23.86 

" 

0 

24.3 

tt 

(Schreinemakers  and  Cocheret,  Chem. 
Weekbl.  1905,  2.  771.) 

(NH4)2SO4+MnSO4. 

Solubility  of  (NH4)2SO4+MnS04  in  H2O. 
G.  per  100  g.  sat.  solution. 


Temp.  =30°. 


MnSO4     (NHi)2SO, 


39.3 
38.49 

33.44 

22.06 

9.02 

2.91 

1.75 

1.77 
0 


0 
3.64 

4.91 

9.65 

20.36 

37.42 

42.58 

43.24 
43.4 


Solid  phase 


MnSO4,  5H2O 
MnSO4,  5H2O+MnS04, 
(NH4)2S04,  6H20 


MnSO4,  (NH4)2SO4,  6H2O 
+(NH4)2S04 

fNH4)2S04 


Temp.  =50°. 


36.26 

0 

MnSO4|  H2O 

35.35 

2.95 

MnSO4,  H2O+2MnS04, 

(NH4)2S04 

30.57 

5.14 

2MnSO4,  (NH4)2SO4 

16.86 

17.62 

M 

6.92 

35.98 

w 

6.29 

39.71 

« 

5.70 

43.24 

2MnSO4,  (NH4)2SO4+ 

(NH4)2S04 

3.49 

44.02 

(NH4)2S04 

0 

45.7 

it 

(Schreinemakers, 


Chem.    Weekbl.    1909,    6. 
131.) 


SULPHATE,  AMMONIUM 


929 


(NH4)2SO4+K2SO4. 

100  pts.  (NH4)2SO4+K2SO4+Aq  sat. 
16.17°  contain  38.41  pts.  of  the  two  salts 
of  which  5.45  pts.  are  K2SO4,  and  32.96  pts 
(NH4)2SO4.  (v.  Hauer,  J.  pr.  28. 137.) 

100  pts.  H2O  dissolve  50.6  pts.  (NH4)2SO 
and  7.2  pts.  K2SO4  at  11.°  (Mulder,  J.  B 
1866.  67.) 

(NH4)2S04  and  K2SO4  replace  each  other  in 
solution,  so  that  by  adding  one  of  these 
salts  to  a  seemingly  saturated  solution  of  the 
other,  it  is  dissolved  with  pptn.  of  the  other 
salt.  (RUdorff,  B.  6.  485.) 


Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  826.) 

Insol.  in  absolute  alcohol.  Sol.  in  500  pts 
alcohol  of  0.872  sp.  gr.,  and  in  62.5  pts.  of 
0.905.  sp.  gr.  (Anthon,  J.  pr.  14.  125.) 

Sol.  in  217.4  pts.  of  66.8%  alcohol  (sp.  gr.  = 
0.88)  at  24.3°.  (Pohl,  J.  pr.  66.  219.) 

Tolerably  sol.  in  alcohol,  the  sp.  gr.  of  which 
is  greater  than  0.860.  Insol.  in  alcohol  of  sp. 
gr.  less  than  0.850. 


Solubility  in  dil.  alcohol. 


Solubility  of  (NH4)2SO4+K2SO4  at  19.1°. 

When  (NH4)2SO4  is  dissolved  in  dil.  alcohol, 
two  layers  are  formed,  the  compositions  of 
which  are  as  follows: 

Solution 

&§ 

« 

6 
? 

^s 

£ 

Sp.  gr. 

Lower  layer 
100  ccm.  contain  in  g. 

Both  salts  in  excess 
15  cc.  sat.  sol.+4g.  K2SO4 
15  cc.  sat.  sol.  +4  g.  (NH4)2SO4 

39.3 
4.94 
2.05 

37.97 
33.26 
40.80 

alcohol 

water 

salt 

.2240 
.1775 
.1661 
.1655 
.1735 

8.'85 
10.62 
11.29 
11.42 

71.43 

68.26 
67.70 
67.34 
66.54 

74.16 
59.54 
56.56 
56.30 
59.20 

(Rudorff,  B.  6.  482.) 

Solubility  of  (NH4)2SO4+K2SO4  in  H2O  at 
25°. 

Sp.  gr. 

Upper  layer 
100  ccm.  containing. 

g.  K2S04 
perl. 

g.(NH^2SOi 
par  1. 

g.  KaSCh 
p^r  1. 

g.  (NH4)2S04 
per  1. 

alcohol 

water 

salt 

0.9530 
0.9512 
0.9440 
0.9098 
0.8750 
0.8549 
0.8308 

41.37 
44.20 
44.27 
52.64 
62.61 
67.04 
77.55 

48.47 
45.95 
45.61 
36.78 
24.60 
18.36 
5.53 

5.45 
4.97 
4.51 
1.56 
0.30 
0.09 
0.00 

127.9 
135.7 

84.2 

0.0 
115.7 

281  .  1 

59.28 
40.27 
0.0 

355.0 

482.7 
542.3 

Results  are  also  given  for  14°,  15°,  16°,  30°, 
46°  and  47°. 
(Tock.  Z.  Krvst.  Min.  1897.  28.  365.) 

(NH4)2S04+Th(S04)2. 
Solubility  of  (NH4)2SO4+Th(SO4)2  at  16< 
Pts.  per  100  pts.  H2O. 


(Bodlander,  Z.  phys.  Ch.  7.  3,  8.) 


Solubility  in  ethyl  alcohol  +Aq. 


(NH4)2SO< 

I 

J3 

h 

Solid  phase 

Upper  layer 

Temp. 

g.  H20 

g.  alcohol 

g.  salt 

2.13 
4.80 
10.02 
16.56 

28.00 
35.20 

15.14 
49.05 

>2.88 
39.74 

3.361 
5.269 

8.947 
13.330 

10.359 
9.821 

6.592 
5.750 
4.583 
1.653 

Th(SO4)2.9H2O 
Tt 

(t 

Th(SO4)2,  9H2O+Th(SO4)2, 
(NH4)2SO4.4H2O 
TMSO4)2.  (NH4)2SO4.4H2O 
"  +Th(S04)2,  2(NH4)2S04. 
2H2O 
Th(SO4)2,  2(NH4)2S04.2H2O 

Th(S04)2,  3(NH4)2S04.3H20 

16.6° 

33.0° 
41.8° 
55.7° 

52.80 
47.99 
47.34 
45.90 

40.21 
46.75 
47.67 
49.47 

6.99 
5.26 
4.99 
4.63 

Lower  layer 

16.6° 
33.0° 
41.8° 
55.7° 

60.33 
61.02 
61.16 
61.59 

10.19 
9.80 
9.74 
9.46 

29.48 
29.18 
29.10 

28.95 

(Traube,  Z.  phys.  Ch.  1887,  1.  509.) 

(Barre,  A.  ch.  1911,  (8)  24.  239.)         *« 

930 


SULPHATE,  AMMONIUM  HYDROGEN 


Solubility  of  (NH4)2SO4  in  alcohol  at  30°. 
Two  liquid  layers  are  formed  between  al- 
cohol concentrations  of  5.8  and  62°. 
Composition  of  layers. 

Solubility  in  propyl  alcohol  +Aq  at  20°. 

%  propyl  alcohol 

%  (NH  4)2SO  4 

20 

30 
40 
50 
60 
70 

6.7 
4.8 
3.2 
2.0 
1.0 
0.4 

Upper  layer 

Lower  layer 

W(;HN) 

% 

«! 

it 

4 

1 

Ml 

(Linebarger,  Am.  Ch.  J.  1892,  14.  380.) 

100  g.  95%  formic  acid  dissolve  25.4  g. 
(NH4)2SO4  at  16.5°.    (Aschan,  Ch.  Ztg.  1913, 
37.  1117.) 
Insol.  in  acetone.     (Eidmann,  C.  C.  1899, 
II.    1014;    Naumann,  B.   1904,    37.    4329). 
Insol.  in  methyl  acetate.     (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.     (Naumann, 
B.  1910,  43.  314.) 
Insol.  in  CS2.    (Arctowski,  Z.  anorg.  1894, 
6.  257.) 

2.2 
2.6 
3.4 
13.2 
17 

56.6 
54.5 
52.3 
31.8 
25 

41.2 
42.9 
44.3 
55 

58 

37.1 
35.7 
33.8 
21.7 
17 

5.8 
6.3 
7.4 
18.4 
25 

57.1 

58 
58.8 
59.9 

58 

At    concentration    of    62%    alcohol,    the 
liquid   is  homogeneous   and   contains   1.3% 
(NH4)2S04. 
(Wibaut,  Chem.  Weekbl.  1909,  6.  401.) 

Solubility  of  (NH4)2S04  in  alcohol  at  60°. 


%  (NH4)2SO4 

%  alcohol 

%H20 

43.02 
41.1 

2.32 
4.1 

54.66 

54.8 

1.2 
0.2 

64^5 
75.5 

34~3 
24.3 

Between  4.1°  and  64.5°,  two  liquid  layers 
are  formed. 

Composition  of  layers. 


Upper  layer 

Lower  layer 

6 

1 

"o 

fa 

J 

B 
g 

*i 

"us 

oo 

1.2 
1.6 
3.8 
7.4 
10 

64.5 
60 
50 
40 
34.4 

34.3 
38.4 
46.2 
52.6 
55.6 

41.1 
36.8 
30.8 
26.6 
23.6 

4.1 
6 
9 
12 
15 

54.8 
57.2 
60.2 
61.4 
61.4 

(Schreinemakers,  Z.  phys.  Ch.  1907,  59.  641.) 
Solubility  in  alcohol  +Aq  at  0°. 


%  (NH4)2SO4 

%  alcohol 

%H20 

41.4 
30.0 

0 

9.41 

58.6 
60.59 

'6.i4 

73^03 

26  '83 

Two  layers   are  formed  between   alcohol 
concentrations  of  9.41  and  73.03%. 
(de  Waal,  Dissert.  1910.) 


Ammonium  hydrogen   sulphate,   NH4HSO4. 

SI.  deliquescent.     Sol.  in  1  pt.  cold  H20. 
(Link.) 

Very  si.  sol.  in  alcohol.    (Gerhardt,  A.  ch. 
(3)  20.  255.) 

Insol.   in  acetone.     (Naumann,   B.    1904, 
37.  4329;  Eidmann,  C.  C.  1899,  II,  1014.) 

(NH4)3H(SO4)2.     Not  deliquescent.     Sol. 
in  H2O.     (Mitscherlich,  Pogg.  39.  198.) 

(NH4)2SO4,  3H2SO4.)    D'Ans  and  Schreiner, 
Z.  anorg.  1913,  80.  241.) 


Ammonium   pz/rosulphate,    (NH4)2S2O7. 
Decomp.  by  H2O.    (Schulze.) 
NH4HS2O7.      (D'Ans    and    Schreiner, 

anorg.  1913,  80.  241.) 


Z. 


Ammonium  ocfosulphate,   (NH4)2S8O26. 
Decomp.  by  H2O.     (Weber,  B.  17.  2497.) 

Ammonium  antimony  sulphate, 

(NH4)2SO4,Sb2(SO4)3. 

Behaves  toward  H2O  and  abs.  alcohol  as 
a  mixture  of  the  components.  (Metzl,  Z. 
anorg.  1805,  48.  152.) 

Decomp.  very  slowly  by  H2O.  (Gut- 
mann,  Arch.  Pharm.  1898,  236.  479.) 

Ammonium  bismuth  sulphate,  NH4Bi(SO4)2 

+4H20. 

Easily  sol.  in  HC1,  and  HNO3+Aq;  less 
sol.  in  cone.  H2SO4,  and  hot  dil.  acids.  Slowly 
decomp.  by  cold  HC2H3O2,  and  dil.  H2SO4  + 
Aq..  (Liiddecke,  A.  140.  277.) 

Ammonium  cadmium  sulphate,  (NH4)2SO4. 
CdSO4+6H2O. 

Can  be  recrystallised  from  a  little  H20 
(v.  Hauer.) 

1  1.  H2O  dissolves  723  g.  anhydrous  sal 
at  25°.  (Locke,  Am.  Ch.  J.  1902,  27.  459.) 


SULPHATE,  AMMONIUM  CHROMIC 


931 


3(NH4)2SO4,  CdSO4+10H2O.  (Andre,  C. 
R.  104.  987.) 

Ammonium  calcium  sulphate, 

(NH4)2Ca(SO4)2+H2O. 

Decomp.  by  H20.  (Fassbender,  B.  11. 
1968.) 

Sol.  in  (NH4)2SO4+Aq.  (Rose,  Pogg. 
110.  292.) 

pfcThis  double  salt  is  stable  between  0°  and 
100°  in  solutions  containing  an  excess  of 
.(NH4)2SO4.  It  is  not  formed  if  the  solution 
contains  less  than  35%  (NH4)2SO4.  (Barre, 
C.  R.  1909,  148.  1605.) 

(SO4)3Ca2(NH4)2.      Decomp.      by     H2O. 
CD'Ans,  B.  1907,  40.  192.) 
pkThis  double  salt  is  formed  in  the  presence 
of  an  excess  of  CaSO4  and  at  temp,  above  80°. 
(Barre,  C.  R.  1909,  148.  1605.) 

Ca5(NH4)2(SO4)6'+H2O.  Decomp.  by  H2O. 
(D'Ans,  B.  1907,  40.  192.) 

Ammonium  calcium  cupric  sulphate, 

Ca2Cu(NH4)2(SO4)4+2H2O. 
Very  stable.    (D'Ans,  B.  1908,  41.  1778.) 

Ammonium  calcium  potassium  sulphate, 

NH4CaK(SO4)2  +H2O. 
Decomp.  by  cold  H2O.     (Fassbender,  B. 
11.  1968.) 

Ammonium  cerous  sulphate,  (NH4)2Ce2(SO4)4 
+8H2O. 

More  sol.  in  cold  than  in  hot  H2O.  (Czud- 
nowicz). 

100  g.  H2O  dissolve  at: 
22.3°  22.35°  35.1°  45.2° 
5.331  5.328    5. 184  4.993  g.  anhydrous  salt, 

45°       55  3°     55  2° 
2 . 994     2 . 240     2 . 187  g.  anhydrous  salt, 

75.4°         85.2° 

1 . 482         1 . 184  g.  anhydrous  salt. 
(Wolff,  Z.  anorg.  1905,  45.  102.) 

5(NH4)2SO4,  Ce2(SO4)3.  (Barre,  C.  R. 
1910,  151.  873.) 

Ammonium   eerie    sulphate,    3(NH4)2SO4, 
Ce(SO4)2+4H2O. 

Slightly  efflorescent.  Easily  sol.  in  H2O. 
(Mendelejeff,  A.  168.  50.) 

3(NH4)2SO4,  2Ce(SO4)2+3H2O.  SI.  sol. 
in  H2O.  (Mendelejeff.) 

Ammonium  chromous  sulphate,  NH4Cr(SO4)2. 

0.407  g.  mol.  anhydrous  salt  is  sol.  in  1  1. 
H2O  at  25°.  (Locke,  Am.  Ch.  J.  1901,  26. 
175.) 

+6H2O.  100  ccm.  of  sat.  aqueous  solution 
contain  55  g.  of  the  salt  at  20°.  Insol.  in 
alcohol.  (Laurent,  C.  R.  1911,  131.  112.) 


Ammonium    chromic    sulphate,    (NH4)2SO4, 
Cr2(S04)3. 

Not  attacked  by  boiling  H2O  or  cone.  HC1 
+Aq.  Very  slowly  attacked  by  boiling  KOH 
-j-Aq  (sp.  gr.  =  1.3).  Insol.  in  CrCl2+Aq  or 
SnCl2+Aq.  (Klobb,  Bull.  Soc.  (3)  9.  664.) 

+5H20.  Is  ammonium  chromosulphate, 
which  see. 

+24H2O.    Chrome  Alum. 

Violet  modification.  Efflorescent.  Sol.  in 
cold  H2O,  but  solution  is  decomp.  on  heating 
with  formation  of  green  modification.  The 
dil.  solution  of  green  modification  is  grad- 
ually converted  into  violet  modification  by 
standing.  Alcohol  ppts.  it  from  aqueous 
solution.  (Schr6tter,  Pogg.  53.  526.) 

100  cc.  H2O  dissolve  10.78  g.  anhydrous,  or 
21.21  g.  hydrated  salt  at  25°.  Melts  in  crystal 
H2O  at  45°.  (Locke,  Am.  Ch.  J.  1901,  26. 174.) 

Solubility  in  HaO. 

Saturation  is  very  slowly  reached  owing  to 
transition  between  violet  and  green  modifi- 
cations.    If  time  of  saturation  is  taken ,  at 
2l/2  hours,  100  g.  of  the  solution  contain  at: 
0°         30°        40° 

3.77      10.6       15.5  g.  (NH4)2Cr2(SO4)4. 

This  is  assumed  to  be  the  solubility  of  the 
violet  modification. 

In  300  hours,  15.96  g.  salt  are  dissolved 
at  30°,  and  24.64  g.  in  250  hours  at  40°. 
(Koppel,  B.  1906,  39.  3741.) 

Calc.  from  electrical  conductivity  measure- 
ments, a  solution  containing  3.8  g.  of  the 
sulphate  in  100  g.  contains  48%  of  the  green 
compound  at  40°  and-  61%  at  55°.  With 
solutions  of  6-7  times  the  above  concentra- 
tion equilibrium  is  reached  at  40°  with  30- 
40%  green  alum.  (Koppel.) 

Sp.  gr.  of  aqueous  solution  of  violet  modi- 
fication at  15°,  containing: 

4  8       12%  (NH4)2Cr2(SO4)4+24H2O. 

1.020  1.0405  1.0610 

Sat.  solution  at  15°  has  sp.  gr.  =  1.070. 
(Gerlach.) 

Green  modification.  Sol.  in  H2O  and  al- 
cohol. When  in  aqueous  solution,  it  gradually 
changes  to  violet  modification. 

Sp.  gr.  of  aqueous  solution  of  green  modi- 
fication at  15°,  containing: 

10  20  30%  (NH4)2Cr2(S04)4+24H2O, 
1.044  1.091  1.142 

40  50  60%  (NH4)2Cr2(S04)4+24H20, 
1.197  1.255  1.317 

70  80  90%.(NH4)2Cr2(SO4)4+24H2O. 
1.384  1.456  1.532 

(Gerlach,  Z.  anal.  28.  498.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

3(NH4)2SO4,  Cr2(SO4)3.  Only  si.  attacked 
by  boiling  H2O.  Not  attacked  by  boiling 
cone.  (NH4)2SO4+Aq.  (Klobb,  Bull.  Soc. 
(3)  9.  663.) 


932 


SULPHATE,  AMMONIUM  COBALTOUS 


Ammonium  cobaltous  sulphate, 

(NH4)2Co(SO4)2+6H2O. 
100  pts.  H2O  dissolve  at: 
0°     10°    18°    23°    35° 
8.9  11.6  15.2  17.1   19.6  pts.  anhydrous  salt, 

40°    45°  50°    60°    75° 
22.3    25  28.7  34.5  43.3  pts.  anhydrous  salt. 
(Tobler,  A.  96.  193.) 

100  pts.  saturated  solution  contain  at: 
20°       40°        60°       80° 
14.9      20.8      25.6      33  pts.  anhydrous  salt. 
(v.  Hauer,  J.  pr.  74.  433.) 

Solubility      of      (NH4)2Cu(SO4)2,      6H2O  + 
(NH4)2Ni(SO4)2,  6H2O  in  H2O  at  13-14°. 
Mols.  per  100  mols.  H2O. 

Cu  salt 

Ni  salt 

%  Cu  salt  in 
solid  phase 

0 
0.1476 
0.2664 
0.4165 
0.4785 
1.0350 

0.521 
0.295 
0.2089 
0.1449 
0.1202 
0 

0 
10.29 
30.59 
52.23 

78.80 
100 

(Fock,  Z.  Kryst.  Min.  1897,  28.  365.) 

1  1.  H2O  dissolves  147.2  g.  anhydrous  salt 
at  25°.  Tobler's  results  are  inaccurate. 
(Locke,  Am.  Ch.  J.  1902,  27V  459.) 

Pptd.  from  aqueous  solution  by  alcohol. 

Ammonium  cobaltic  sulphate, 

(NH4)2Co2(S04)4+24H20. 


Sol.    in    H2O    with 
Chem.  Soc.  59.  760.) 


decomp.      (Marshall, 


Ammonium  cobaltous  cupric  sulphate, 

2(NH4)2SO4,  CoSO4,  CuSO4  +  12H2O. 
Quite  easily  sol.  in  hot  H2O,  but  on  long 
boiling  a  basic  salt  is  pptd.    (Vohl,  A.  94.  58.) 

Ammonium  cobaltous  ferrous  sulphate, 

2(NH4)2SO4,  CoSO4,  FeSO4+12H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 

Ammonium  cobaltous  magnesium  sulphate, 

2(NH4)SO4,  CoSO4;  MgSO4  +  12H2O. 
Sol.  in  H2O.    (Vohl,  A-  94.  57.) 

Ammonium  cobaltous  manganous  sulphate, 

2(NH4)SO4;  CoSO4,  MnSO4+12H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 

Ammonium  cobaltous  nickel  sulphate, 

2(NH4)SO4,  CoSO4,  NiSO4+12H2O. 
Sol.  in  H20.    (Vohl,  A.  94.  57.) 

Ammonium  cobaltous  zinc  sulphate, 

2(NH4)2SO4,  CoSO4,ZnSO4  +  12H2O. 
Sol,  in  H20.    (Vohl,  A.  94.  57.) 

Ammonium  cupric  sulphate,  (NH4)2SC4, 

CuSO4+6H2O. 
Efflorescent  in  warm  air. 

Sol.  in  1.5  pts.  boiling   H2O,   and  separates  almost 
wholly  on  ccoling.     (.Vogel,  J.  pr.  2.  194 
Sol.  in  1.55  pts.  H2O  at  18.75°.     (Abl.) 

100  pts.  H2O  at  19°  dissolve  26.6  pts.,  and 
sat.  solution  has  sp.  gr.  =  1.1337.  (Schiff,  A. 
109.  426. 

100  g.  sat.  solution  at  30°  contain  30.36  g. 
anhydrous  salt.  (Schreinemakers,  Arch.  Ne'er. 
Sci.  1910,  (2)  16.  92.) 


K  salt 

NH4  salt' 

%  K  salt  in 
solid  phase 

0 

1.035 

0 

0.897 

0.8618 

5.06 

0.2269 

0.6490 

16.76 

0.2570 

0.5887 

30.40 

0.2946 

0.5096 

36.63 

0.3339 

0.3319 

50.15 

0.4560 

0.1961 

69.93 

0.4374 

0 

100. 

Solubility      of      (NH4)2Cu(SO4)2,      6H2O  + 
K2Cu(SO4)2,  6H2O  in  H2O  at  13-14°. 
Mols.  per  100  mols.  H2O. 


(Fock.) 

Solubility      of      (NH4)2Cu(SO4)2,      6H2O  + 

(NH4)2Zn(SO4),  6H2O  in  H2O  at  13-14°. 

Mols.  per  100  mols.  H2O. 


Cu  salt 

Zn  salt 

%  Cu  salt  in 
solid  phase 

0.0422 
0.0666 
0.1218 
0.2130 
0.3216 
1.035 

0.8069 
0.5638 
0.5115 
0.4924 
0.4022 
0 

2.39 
4.52 
9.03 
14.67 
22.62 
100. 

(Fock.) 

(NH4)2SO4,   2CuSO4.      Very  sol.   in  H2O 
(Klobb,  C.  R.  115.  220.) 

Ammonium  cupric  ferrous  sulphate. 

Sol.  in  H2O  without  decomposition.    (Vohl, 
A.  94.  61.) 

Ammonium  cupric  magnesium  sulphate, 

2(NH4)2SO4,  CuSO4,  MgSO4  +  12H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 

Ammonium  cupric  magnesium  potassium  sul- 
phate, (NH4)2SO4,  CuSO4,  MgSO4,  K2S04 
+12H20. 

Sol.  inH2O.    (Schiff.) 
2(NH4)2SO4,    CuSO4,    2MgSO4,    K2SO4+ 
18H2O.    Sol.  inH2O.    (Schiff.) 


SULPHATE,  AMMONIUM  IRON 


933 


Ammonium  cupric  manganous  sulphate, 

2(NH4)2SO4,  CuSO4,  MnSO4  +  12  H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 

Ammonium  cupric  nickel  sulphate, 

2(NH4)2SO4,  CuSO4,  NiSO4  +  12H2O. 
Sol.  in  H2O.    (Vohl.) 

Ammonium  cupric  potassium  sulphate, 

NH4KSO4,  CuSO4+6H2O. 
Sol.  inH2O.    (Schiff.) 

Ammonium  cupric  zinc  sulphate, 

2(NH4)2SO4,  CuSO4,  ZnSO4+12H2O. 
Sol.  inH2O.    (Vohl.) 

Ammonium  cupric  sulphate  ammonia, 

(NH4)2SO4,  CuO,  2NH3. 
Sol.  in  1.5  pts.  cold  H2O,  but  decomp.  on 
exposure  to  air  or  dilution.    Insol.  in  alcohol. 
(Kuhn.) 

Ammonium  didymium  sulphate,  (NH4)2S04, 
Di2(SO4)3+8H2O. 

Sol.  in  18  pts.  H2O,  and  less  easily  in 
(NH4)2SO4+Aq.  (Marignac.) 

Moderately  sol.  in  H2O.  (Cleve,  Bull.  Soc. 
(2)  43.  362.) 

Ammonium  erbium  sulphate,  (NH4)2SO4, 

Er2(SO4)3+8H2O. 
Sol.  inH2O.    (Cleve.) 

Ammonium  gallium  sulphate, 

(NH4)2Ga2(SO4)4+24H2O. 

Sol.  in  cold  water  and  dilute  alcohol.    Cone. 

solution  clouds  up  on  boiling,  but  clears  on 

cooling.     Dil.  solution  separates  out  a  basic 

salt,  insol.  in  hot  or  cold  H2O.    (Boisbaudran.) 

Ammonium  glucinum  sulphate,   (NH4)2SO4, 

G1S04+2H20. 
Sol.  in  H2O.    (Atterberg.) 


Ammonium  indium  sulphate, 

(NH4)2In2(SO4)4+24H2O. 

100  pts.  H2O  dissolve  200  pts.  salt  at  16°, 
and  400  pts.  at  30°. 

Insol.  in  alcohol. 

Melts  in  crystal  H2O  at  36°.  (Rossler,  J. 
pr.  (2)  7.  14.) 

+8H2O.    (Rossler.) 

Ammonium    iridium    sulphate,    (NH4)2SO4, 

Ir2(S04)3+24H20. 

Easily  sol.  in  H2O.  (Marino,  Z.  anorg. 
1904,  42.  221.) 

Ammonium  iron  (ferrous)  sulphate, 

(NH4)2Fe(S04)2+6H20. 
Much  less  sol.  in  H2O  than  FeSO4+7H2O. 
(Vogel,  J.  pr.  2.  192.) 


100  pts.  H2O  dissolve  at: 
0°     12°    20°    30°    36° 
12.2  17.5  21.6  28.1  31.8  pts.  anhydrous  salt, 

45°    55°    60°    65°    75° 
36.2  40.3  44.6  49.8  56.7  pts.  anhydrous  salt. 
(Tobler,  A.  95.  193.) 

100  pts.  H2O  at  16.5°  dissolve  35.9  pts. 
hydrous  salt. 

1 1.  H2O  dissolves  351  pts.  or  1.044  g.  mol. 
anhydrous  salt  at  25°.  (Locke,  Am.  Ch.  J. 
1902,  27.  459.) 

Sol.  in  H2O  without  decomp.  Aq.  solution 
at  30°  contains  13.13%  FeSO4  and  11.45% 
(NH4)2SO4.  (Schreinemakers,  C.  C.  1910,  I. 
801.) 

Sp.  gr.  of  (NH4)2FeSO4+Aq  at  19°. 

%  =  %(NH4)2FeS04+6H20. 


% 

Sp.  gr. 

% 

Sp.  gr. 

% 

Sp.  gr. 

1 

1.006 

11 

.066 

21 

1.130 

2 

1.013 

12 

.073 

22 

.136 

3 

1.018 

13 

.080 

23 

.143 

4 

1.024 

14 

.085 

24 

.150 

5 

1.030 

15 

.092 

25 

.156 

6 

1.036 

16 

.097 

26 

.164 

7 

1.042 

17 

.104 

27 

.171 

8 

1.047 

18 

.110 

28 

1.179 

9 

1.054 

19 

1.116 

29 

1.185 

10 

1.060 

20 

1.124 

30 

1.193 

(Schiff  calculated    by  Gerlach,   Z.   anal.   8. 
280.) 

Insol.  in  acetone. 

Ammonium  ferric  sulphate,  basic. 

Extremely  difficultly  sol.  in  HCl+Aq.  Not 
decomp.  by  KOH+Aq.  (Berzelius.) 

5(NH4)2O,  3Fe2O3,  12SO3+18H2O  or 
2(NH4)2O,  Fe2O3,  4SO3+4H2O.  Sol.  in  2.4 
pts.  cold  H2O.  (Maus,  Pogg.  11.  79.) 

Ammonium  iron  (ferric)  sulphate,  (NH4)2SO4, 
Fe2(S04)3. 

Attacked  slowly  by  cold  H2O.  (Lachaud 
and  Lepierre.) 

Nearly  insol.  in  H2O.  (Wemland,  Z.  anorg. 
1913,  84.  363.) 

+24H2O.  Iron  alum.  Sol.  in  3  pts.  H2O 
at  15°.  (Forchhammer,  Ann.  Phil.  6.  406.) 

100  cc.  H2O  dissolve  44.15  g.  anhydrous,  or 
124.40  g.  hydrated  salt  at  25°,  or  1.659  g. 
mols.  anhydrous  salt  are  sol.  in  1  1.  H2O  at 
25°.  (Locke,  Am.  Ch.  J.  1901,  26.  174.) 

Sp.  gr.  of  aqueous  solution  at  15°  contain- 
ing: 

5  10  15%  (NH4)2Fe2(S04)4+24H20, 
1.023  1.047  1.071 

20  25  30%  (NH4)2Fe2(S04)4+24H20, 
1.096  1.122  1.148 

35         40%  (NH4)2Fe2(S04)4+24H20. 
1.175     1.203 


934 


SULPHATE,  AMMONIUM  IRON 


40%  solution  is  sat.  at  15°.     (Gerlach,  Z. 

anal.  28.  496.) 

Melts  in  crystal  H2O  at  40°.    (Locke.) 
3(NH4)2SO4,    Fe2(SO4)?.      Insol.    in    cold 

H2O.    (Lachaud  and  Lepierre.) 

Ammonium  iron  (ferroferric)   sulphate, 

4(NH4)2SO4,  FeSO4,  Fe2(SO4)3+3H2O. 
SI.  sol.  in  .cold  H2O;  decomp.  into  basic  salt 
by  hot  H2O;  insol.  in  alcohol.    (Lachaud  and 
Lepierre,  C.  R.  114.  916.) 

Ammonium    ferrous    magnesium    sulphate, 

4(NH4)2SO4,  3FeSO4,  MgSO4+24H2O. 
Sol.  in  H2O.    (Schiff,  A.  107.  64.) 
2(NH4)2SO4,  FeSO4,  MgSO4+12H2O.    Sol. 
in  H2O.    (Vohl,  A.  94.  57.) 

Ammonium  ferrous  manganous  sulphate, 

•  2(NH4)2SO4,  FeSO4,  MnS04+12H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 

Ammonium  ferrous  nickel  sulphate, 

2(NH4)2S04,  FeS04,  NiSO4+12H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 

Ammonium  ferrous  zinc  sulphate, 

2(NH4)2S04,  FeS04,  ZnSO4+12H2O. 
Sol.  in  H2O.    (Bette,  A.  14.  286.) 

Ammonium  lanthanum  sulphate,  (NH4)2SO4, 
La2(SO4)3+8H2O. 

SI.  sol.  in  H2O.    (Marignac.) 

Quite  sol.  in  H2O.    (Cleve.) 

+2H2O.    (Barre,  C.  R.  1910,  161.  872.) 

5(NH4)2SO4,  2La2(SO4)3.  SI.  sol.  in 
(NH4)2SO4+Aq  of  concentrations  above  60%. 
(Barre,  A.  ch.  1911,  (8)  24.  246.) 

5(NH4)2SO4,  La2(SO4)3.    (Barre.) 

Ammonium  lead  sulphate,  (NH4)2SO4,  PbSO4. 

Decomp.  by  H2O  into  its  constituents. 
(Wohler  and  Litton,  A.  43.  126.) 

Decomp.  by  H2O.  Only  stable  in  contact 
with  solutions  containing: 

13.86  pts.  (NH4)2SO4  per  100  pts.  H2O  at 
20°. 

19.25  pts.  (NH4)2SO4  per  100  pts.  H2O  at 
50°. 

24.31  pts.  (NH4)2SO4  per  100  pts.  H2O  at 
75°. 

29.42  pts.  (NH4)2SO4  per  100  pts.  H2O  at 
100°. 

(Barre,  C.  R.  1909,  149.  294.) 

Ammonium  lithium  sulphate,  NH4LiSO4. 

Solubility  in  H2O  =  35.25%  at  —10,°  and 
36.18%  at  70°.  (Schreinemakers,  C.  C.  1906, 
I.  217.) 

This  is  the  only  double  salt  which 
(NH4)2S04  forms  with  Li2SO4  below  100°. 
(Spielrein,  C.  R.  1913,  167.  48.) 


Ammonium  magnesium  sulphate, 

(NH4)2Mg(SO4)2+6H2O. 
100  pts.  H2O  dissolve  15.9  pts.  anhydrous 
double  salt  at  13°.    (Mulder.) 
100  pts.  H2O  dissolve  at: 
0°    10°    15°    20°    30° 
9.0  14.2  15.7  17.9  19.1  pts.  anhydrous  salt, 

45°    50°    55°    60°    75° 
25.6  30.0  31.9  36.1  45.3  pts.  anhydrous  salt. 
(Tobler,  A.  96.  193.) 

More  sol.  in  H2O  than  (NH4)2SO4  or  MgSO4 
(Graham.) 

1  1.  H2O  dissolves  199  pts.  anhydrous  salt 
at  25°.  Tobler's  results  are  inaccurate. 
(Locke,  Am.  Ch.  J.  1902,  27.  459.) 

100  g.  H2O  dissolve  at: 
34°  41°  F. 

18.22         20.72  g.  (NH4)2SO4,  MgSO4,  6H2O. 

50°  59°  F. 

22.48         24.08  g.  (NH4)2SO4,  MgSO4,  6H2O, 

60°  70°  F. 

24.81         28.26  g.  (NH4)2SO4,  MgSO4,  6H2O, 

81°  F. 

33.33  g.  (NH4)2S04,  MgSO4,  6H2O. 
(Lothian,  Pharm.  J.  1910,  (4)  30.  546.) 

Lothian's  results  for  solubility  in  H2O 
probably  incorrect  because  of  inaccuracy  of 
experimental  method.  (Seidell,  Pharm.  J. 
1911,  (4)  33.  846.) 

Solubility  of  (NH4)2Mg(SO4)2  in  H2O  at  t°. 


t 

g.  anhydrous  salt  par  103  g. 

solution 

H20 

0 

10.58 

11.83 

10 

12.75 

14.61 

20 

15.23 

17.96 

25 

16.45 

19.69 

30 

17.84 

21.71 

40 

20.51 

25.86 

50 

23.18 

30.17 

60 

26.02 

35.17 

80 

32.58 

48.32 

100 

39.66 

65.72 

(Porlezza,  Att.  Ace.  Line.  1914,  (5)  23.  II, 

509.) 
Min.  Cerbolite. 

Ammonium  magnesium  nickel  sulphate, 

2(NH4)2S04,  MgS04,  NiS04+12H20. 
Sol.  in  H20.    (Vohl,  A.  94.  57.) 

Ammonium  magnesium  potassium  zinc  sul- 
phate,  2(NH4)2SO4,    3MgSO4,    3K2SO4, 
2ZnSO4+30H2O. 
Sol.  in  H2O.    (Schiff,  A.  107.  64.) 
(NH4)2S04,    2MgS04,    2K2S04,    ZnSO4  + 
18H2O.    Sol.  in  H2O.    (Schiff.) 

(NH4)2S04,  MgS04,  K2S04,  ZnSO4+12H2O 
Sol.  inH2O.    (Schiff.) 


SULPHATE,  AMMONIUM  THALLIC 


935 


Ammonium  magnesium  zinc  sulphate, 

2(NH4)2SO4,  MgSO4,  ZnSO4+12H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 

Ammonium  manganous  sulphate,  (NH4)2SO4 

MnSO4+6H2O. 

Deliquescent.    Easily  sol.  in  H2O.    (Jahn.' 
1  1.  H2O  dissolves  372  g.  anhydrous  sal 

at  25°.    (Locke,  Am.  Ch.  J.  1902,  27.  459.) 
(NH4)2SO4,  2MnSO4.    Readily  decomp.  ty 

H2O.    (Lepierre,  C.  R.  1895,  120.  924.) 

Ammonium  manganic  sulphate,  (NH4)2SO4 
Mn2(S04)3. 

Decomp.  by  H2O.  Insol.  in  ether,  C6H6,  and 
cone.  H2SO4.  Sol.  in  dil.  H2SO4+Aq.  (Le- 
pierre, Bull.  Soc.  1895,  (3)  13.  596.) 

+24H2O.  Decomp.  by  H2O.  (Mitscher- 
lich.) 

Ammonium  manganous  nickel  sulphate, 

2(NH4)2S04,  MnS04,  NiSO4+12H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 

Ammonium  manganous  zinc  sulphate, 

2(NH4)2S04,  MnS04,  ZnSO4+12H2O. 
Sol.  inH2O.    (Vohl.) 

Ammonium  mercuric  sulphate,  (NH4)2SO4, 
3HgS04+2H20. 

(Hirzel,  J.  B.  1860.  333.) 

(NH4)2S04,  HgS04.  Difficultly  sol.  in 
H2O.  Easily  sol.  in  NH4OH+Aq. 

Ammonium   mercurous   sulphate   ammonia, 

3Hg20,  2(NH4)HgS04,  2NH3. 
Insol.  in  hot  or  cold,  dil.  or  cone.  H2S04 
and  HNO3.     Sol.  in  HC1.     (Tarugi,  Gazz. 
ch.  it.  1903,  33.  (1)  131.) 

Ammonium  nickel  sulphate,  (NH4)2SO4, 
NiS04+6H20. 

Sol.  in  4  pts.  cold  H2O.     (Link,  1796.) 

100  pts.  H2O  dissolve  at: 
3.5°    10°    16°    20°    30° 
1.8      3.2     5.8     5.9     8.3  pts.  anhydrous  salt, 

40°    50°    59°    68°    85° 
11.5  14.4  16.7  18.8  28.6  pts.  anhydrous  salt. 
(Tobler,  A.  95.  193.) 

100  pts.  sat.  solution  contain  at  20°,  9.4; 
at  40°,  13.2;  at  60°,  18.6;  at  80°,  23.1  pts. 
anhydrous  salt.  (v.  Hauer,  J.  pr.  74.  433.) 

1  1.  H2O  dissolves  75.7  g.  anhydrous  salt 
at  25°.  (Locke,  Am.  Ch.  J.  1902,  27.  459.) 

Nearly  insol.  in  a  weak  acid  solution  of 
(NH4)2SO4.  (Thompson,  C.  C.  1863.  957.) 

Ammonium  nickel  zinc  sulphate,  2(NH4)2SO4, 

NiS04,  ZnS04+12H20. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 


Ammonium  nickel  sulphate  ammonia, 
(NH4)2SO4,  NiS04,  6NH3+3H2O. 
(Andre,  C.  R.  106.  936.) 

Ammonium   platinic    sulphate.   2(NH4)2SO4, 

Pt3(SO4)3+25H2O. 
Sol.  in  H2O.    (Prost,  Bull.  Soc.  (2)  46. 156.) 

Ammonium  potassium  sulphate,  (NH4)2SO4, 
K2S04+4H20. 

Soluble  in  H2O.  100  pts.  H2O  at  16°  dis- 
solve 13.68  pts.  salt.  (Thomson,  1831.) 

Min.  Taylorite. 

Ammonium  praseodymium  sulphate, 

(NH4)2S04,  Pr2(S04)3+8H20. 
SI.  sol.  in  H2O.     (von  Scheele,  Z.  anorg. 
1898,  18.  359.) 

Ammonium  rhodium  sulphate, 

(NH4)2S04,  Rh2(S04)3+24H20. 
Very  sol.  H2O;  melts  in  crystal  H2O  at 
102-103°.    (Piccini,  Z.  anorg.  1901,  27.  67.) 

Ammonium  samarium  sulphate,  (NH4)2SO4, 

Sm2(S04)3+8H20. 

SI.  sol.  in  H2O.  (Cleve,  Bull.  Soc.  (2)  43. 
166.) 

Ammonium  scandium  sulphate,  (NH4)2S04. 
Sc2(S04)3. 

Sol.  inH2O.    (Cleve.) 

Sol.  in  H2O  and  in  dil.  (NH4)2SO4+Aq. 
(R.  J.  Meyer,  Z.  anorg.  1914,  86.  279.) 

Ammonium  sodium  sulphate,  NH4NaSO4-f 
2H2Q. 

100  pts.  H2O  dissolve  46.6  pts.  of  cryst.  salt 
at  15°,  and  the  solution  has  a  sp.  gr.  of  1.1749. 

Sp.  gr.  of  aqueous  solution  containing: 
31.8     24.44     15.9%  NH4NaSO4+2H2O, 
1.17491.1380  1.0849 

12 . 72         6 . 36     %  NH4NaSO4+2H2O. 
1.0679      1.0337 

(Schiff,  A.  114.  68.) 

Ammonium  strontium  sulphate. 

Insol.  in  excess  of  (NH4)2S04+Aq.  (Rose. 
Pogg.  110.  296.) 

(NH4)2S04,  SrS04.  This  double  salt  is 
only  stable  in  contact  with  nearly  sat.  solu- 
tions of  (NH4)2SO4.  (Barre,  C.  R.  1909,  149. 
293.) 

Ammonium  tellurium  sulphate, 

(NH4)HS04,  2Te02,  SO3+2H2O. 
As  K  salt.     (Metzner,  A.  ch.   1898,   (7) 
16.  203.) 

Ammonium  thallic  sulphate,  NH4T1(SO4)2. 
(Marshall,  C.  C.  1902,  II.  1089.) 
+4H20.     Decomp.  by  H2O.     Easily  sol. 

n  dil.  acids.    (Fortini,  Gazz.  ch.  it.  1905.  36. 

2)  450.) 


SULPHATE,  AMMONIUM  THORIUM 


Ammonium  thorium  sulphate,  2(NH4)2SO4, 
Th(S04)2. 

Easily  sol.  in  H2O  and  sat.  (NH4)2SO4+ 
Aq.  (Cleve.) 

+2H2O.    (Barre.) 

(NH4)2SO4,  Th(SO4)2+4H2O.  (Barre,  A. 
ch.  1911,  (8)  24.  240.) 

3(NH4)2SO4,   Th(SO4)2+3H2O.     (B.) 

Ammonium  titanium  sulphate, 
(NH4)2S04,  TiO,  S04+H20. 

Very  sol.  in  H2O  with  decomp. 

Insol.  in  cone.  H2SO4.  (Rosenheim,  Z. 
anorg.  1901,  26.  252.) 

(NH4)2O,  2TiO2,  2SO3+3H2O.  Slowly 
decomp.  by  H2O.  (Blondel,  Bull.  Soc.  1899, 
(3)  21.  262.) 

Ammonium    titanium    ses<??usulphate, 
(NH4)2S04,  3Ti2(S04)3+18H20. 

Insol.  in  H2O;  sol.  in  HC1. 

Insol.  in  H2SO4.  Decomp.  by  boiling  with 
cone.  H2SO4.  (Stabler,  B.  1905,  38.  2623.) 

Ammonium  uranous.  sulphate,  2(NH4)2SO4, 

U(SO4)2. 

Easily  sol.  in  H2O.    (Rammelsberg.) 
Sol.  in  H2O  but  solution  rapidly  decomp. 

(Kohlschiitter,  B.  1901,  34.  3630.) 

Ammonium    uranyl     sulphate,     (NH4)2SO4, 

(UO2)S04+2H2O. 
Quite  difficultly  sol.  in  H2O.    (Arfvedson.) 

Ammonium  vanadous  sulphate, 
fNH4)2SO4,  VSO4+6H2O. 

Decomp.  in  the  air. 

Sol.  in  H2O.  (Piccini,  Z.  anorg.  1899,  19. 
205.) 

Less  sol.  in  H2O  than  VSO4+7H2O.  (Pic- 
cini and  Marino,  Z.  anorg.  1902,  32.  60.) 

Ammonium  vanadic  sulphate, 

(NH4)2S04,  V2(S04)3+12H20. 

Insol.  in  H2O. 

Insol.  in  H2SO4.  Decomp.  by  boiling  with 
cone.  H2SO4. 

Sol.  in  HC1.     (Stabler,  B.  1905,  38.  3980.) 

+24H2O.  Very  sol.  in  H2O;  decomp.  in 
the  air.  (Piccini,  Z.  anorg.  1896,  11.  108.) 

100  pts.  H2O  dissolve  39.76  pts.  salt  at  10°. 

Sp.  gr.  of  sat.  solution  at  4°/20°  =  1.687. 
(Piccini,  Z.  anorg.  1897,  13.  446.) 

1  1.  H2O  dissolves  31.69  g.  anhydrous  or 
78.51  g.  hydrated  salt  at  25°,  or  1.210  g.  mols. 
anhydrous  salt  are  sol.  in  1  1.  H2O  at  25°. 

Mpt.  of  crystals =45°.  (Locke,  Am.  Ch. 
J.  1901,  26.  175.) 

Ammonium  vanadyl  sulphate, 

(NH4)2SO4,  VOSO4+33^H2O. 
Easily  sol.  in  H2O  and  in  a  mixture  of  a  1- 
cohol  and  cone.  H2SO4,  but  cannot  be  recryst. 
therefrom.    (Koppel  and  Behrendt,  Z.  anorg. 
1903,  35.  176.) 


(NH4)2SO4  2VOSO4+H2O.  Deliquescent. 
Slowly  but  abundantly  sol.  in  H2O,  but  can- 
not be  recryst.  from  it  except  by  addition  of 
H2SO4.  (Koppel  and  Behrendt,  Z.  anorg. 
1903,  35.  172.) 

Ammonium   yttrium   sulphate,   2(NH4)2SO4, 

Y2(S04)3+9H20. 
Sol.  inH20.    (Cleve.) 

Ammonium  zinc  sulphate,  (NH4)2SO4,  ZnSO4 

+6H2O. 

100  pts.  H2O  dissolve  pts.  (NH4)2S04, 
ZnSO4  at: 

0°        10°       13°       15°      20° 

7.3      8.8    10.0    12.5    12.6  pts.  salt, 

30°      45°       60°       75°       85° 
16.5    21.7    29.7    37.8    46 . 2  pts.  salt. 
(Tobler,  A.  95.  193.) 

1  1.  H2O  dissolves  140.8  g.  anhydrous 
salt  at  25°.  (Locke,  Am.  Ch.  J.  1902,  27. 
459.) 

+7H2O.    (Andre,  C.  R.  104.  987.) 

Ammonium  zirconium  sulphate. 

Sol.  in  cold  or  hot  H2O  or  in  acids.  (Ber- 
zelius.) 

Ammonium  sulphate  antimony  fluoride, 

(NH4)2SO4,  2SbF3. 

Very  sol.  in  H2O.  (Mayer,  B.  1894,  27. 
R.  922.) 

Ammonium  sulphate  chromic  chloride, 

2(NH4)2SO4,  CrCl3+6H2O. 
Sol.  in  H2O.    (Weinland,  B.  1907, 40.  3768.) 

Ammonium  sulphate  hydrogen  peroxide, 
(NH4)2S04,  H202. 

Efflorescent  in  air. 

Easily  sol.  in  H2O.  (Willstatter,  B.  1903, 
36.  1829.) 

Antimony  sulphate  basic,,  7Sb2O3,  2SO3  + 
3H20. 

Insol.  in,  and  not  decomp.  by  hot  or  cold 
H2O.  (Adie,  Chem.  Soc.  67.  540.) 

5Sb2O3,  2SO3+7H2O.  Insol.  in  H2O. 
(Hensgen,  R.  t.  c.4.401.) 

2Sb2O3,  SO3+xH2O.  Not  decomp.  by 
coldH2O.  (Adie.) 

Sb2O3,  SO3  =  (SbO)2SO4.  Decomp.  by  hot 
H2O.  (Peligot,  J.  B.  1847.  426.) 

+H2O.    As  above.    (Adie.) 

Sb2O3,  2SO3,  and  +H2O,  and  +2H2O. 
Scarcely  decomp.  by  cold,  slowly  by  boiling 
H2O.  Slowly  sol.  in  dil.  HCl+Aq.  (Adie.) 

Antimony  sulphate,  Sb2(SO4)3. 

Very  deliquescent.  Combines  with  H2O  to 
a  hard  mass  with  evolution  of  heat;  with  more 
H2O  it  becomes  liquid,  and  by  repeated  treat- 


SULPHATE,  BARIUM 


937 


merit  with  much  boiling  H2O  it  is  wholly 
decomp.  into  H2SO4  and  Sb2O3.  (Hensgen, 
R.  t.  c.  4.  401.) 

Antimony  sulphate,  acid,  Sb2O3,  4SO3, 
Decomp.  by  H2O.    (Adie.) 
Sb2O3+8,    or   9SO3.      Decomp.    by   H2O. 

(Adie.) 

Antimony  barium  sulphate, 

Sb2(SO4)3,  BaSO4+6H2O. 
As  Ca  comp.     (Kiihl,  Z.  anorg.  1907,  54. 

257.) 

Antimony  caesium  sulphate,  SbCs(SO4)2. 

Slowly  decomp.  by  cold  H2O.  (Gutman, 
Arch.  Pharm.  1908,  246.  188.) 

Antimony  calcium   sulphate, 
Sb2(S04)3,  CaSO4+6H2O. 
Decomp.  by  H2O.     (Kiihl,  Z.  anorg.  1907, 
64.  257.) 

Antimony  lithium  sulphate,  SbLi(SO4)2. 

Decomp.  by  H2O.  (Gutman,  Arch.  Pharm. 
1908,  246.  187.) 

Antimony    potassium    sulphate,    KSb(SO4)2. 
Decomp.     by    H2O.       (Gutmann,     Arch. 
Pharm.  1898,  236.  478.) 

Antimony  rubidium  sulphate,  SbRb(SO4)2. 
Slowly  decomp.  by  cold  H2O.     (Gutman.) 

Antimony  silver  sulphate,  SbAg(SO4)2. 
Slowly  decomp.  by  H2O.    (Kiihl,  Z.  anorg. 

1907,  54.  258.) 

Slowly  decomp.  by  cold  H2O.  (Gutman 
Arch.  Pharm.  1908,  246.  189.) 

Antimony  sodium  sulphate,  NaSb(SO4)2. 

Easily  decomp.  by  H2O.  (Gutmann, 
Arch.  Pharm.  1898,  236.  478.) 

Antimony    strontium     sulphate,     Sb2(SO4)3, 

SrSO,+6H20. 
As  Ca  comp.     (Kiihl,  Z.  anorg.  1907,  54. 

257.) 

Antimony  thallium  sulphate,  SbTl(SO4)2. 

Slowly  decomp.  by  cold  H20.  Decomp. 
by  cone.  H2SO4.  (Gutman,  Arch.  Pharm. 

1908,  246.  189.) 

Arsenic  sulphate. 

See  Arsenic  sulphur  ifn'oxide. 

Barium  sulphate,  BaSO4. 

Sol.  in  43,000  pts.  H2O  (Kirwan) ;  in  200,000  pts.  H2O 
(Margueritte,  C.  R.  38.  308). 

100  pts.  H2O  dissolve  0.002  pt.  BaSO4.  (lire's 
Diet.) 


BaCh+Aq  containing  1  pt.  BaO  to  71,000  pts.  H2O, 
when  treated  with  H2SC>4,  becomes  turbii  in  y>  hour. 
(Harting,  J.  pr.  22.  52.) 

BaCNOah+Aq  containing  1  pt.  BaO  to  25,000  pts. 
H2O  gives  a  distinct  cloud  with  H2SO4  or  Na2SO4+Aq; 
with  50,000-100,000  pts.  H2O  a  slight  turbidity  is 
produced;  with  200,000-400,000  pts.  H2O  the  mixture 
becomes  turbid  in  a  few  minutes;  while  with  800,000 
pts.  H2O  no  action  is  visible.  (Lassaigne,  J  Chim.  Med. 
8.  526.) 

Sol.  in  800,000  pts.  H2O  (Calyert);  in 
400,000  pts.  cold  or  hot  H2O  (Fresenius). 

Calculated  from  the  electrical  conductivity 
of  the  solution,  BaS04  is  sol.  in  429,700  pts. 
H2O  at  18.4°,  and  320,000  pts.  at  37.7°. 
(Holleman,  Z.  phys.  Ch.  12.  131.) 

1  1.  H2O  dissolves  1.72  mg.  at  2°;  1.97  mg. 
at  10°;  2.29  mg.  at  19.0°;  2.60  mg.  at  26°; 
2.91  mg.  at  34°.  CKohlrausch  and  Rose,  Z. 
phys.  Ch.  12.  241.) 

Calculated  from  the  electrical  conductivity 
of  the  solution,  BaSO4  is  sol.  in  425,000  pts. 
H2O  at  18.3°.  Results  of  Fresenius  and 
Hintz  (Z.  anal.  1896,  35.  170)  are  incorrect. 
(Kiister,  Z.  anorg.  1896,  12.  267.) 

Sat.  aq.  solution  contains  2.29  mg.  BaSO4 
per  liter  at  25°  when  particles  of  salt  are  not 
less  than  1.8/u  in  diameter. 

Sat.  aq.  solution  contains  4.15  mg.  BaSO4 
per  liter  at  25°  when  particles  of  salt  are  0.1/i 
in  diameter.  OK  =  0.0001  cm.)  (Hulett,  Z. 
phys.  Ch.  1901,  37.  398-9.) 

In  general  the  influence  of  the  size  of  the 
grain  on  the  solubility  of  the  substance  is 
negligible  when  the  solubility  exceeds  2%. 
The  increase  of  normal  solubility  by  using 
finely  divided  solids,  amounts  to  80%  in  the 
case  of  BaSO4.  (Hulett,  Z.  phys.  Ch.  1904, 
47.  366.) 

1  1.  H2O  dissolves  2.3  mg.  BaSO4  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1904,  50.  356.) 

Calculated  from  electrical  conductivitv  of 
BaSO4+Aq. 

0.0190  milli-equivalents  are  sol.  in  1  liter 
H2O  at  18°;  0.0212  at  25°;  0.0288  at  50°; 
0.0334  at  100°. 

(Melcher,  J.  Am.  Chem.  Soc.  1910,  32.  55.) 

Not  attacked  by  cold  HC1  or  HNO3-f-Aq 
after  several  hours,  and  only  in  traces  after 
several  days.  On  boiling,  traces  of  BaSO4 
dissolve,  and  the  liquid  after  cooling  can  be 
precipitated  by  BaCl2  or  H2SO4+Aq,  but 
not  by  H2O  alone.  (Rose,  Pogg.  95. 
108.) 

By  washing  BaSO4  long  enough  with  H2O 
containing  HC1  or  HNO3  IHC2H3O2  (Siegle)], 
the  filtrate  can  be  precipitated  by  H2SO4  or 
BaCl2.  (Piria,  J.  B.  1856.  334.) 

1000  pts.  3%  HCl+Aq  dissolve  0.06  pt. 
BaSp4  in  the  cold,  and  still  more  on 
boiling. 

230  com.  HCl+Aq  of  1.02  sp.  gr.  dissolve 
0.048  g.  BaSO4  from  0.679  g.  BaS04  when 
boiled  l/£  hour. 

168  com.  HCl-f-Aq  of  1.03  sp.  gr.  dissolve 
0.0075  g.  BaSO4  from  0.577  g.  BaSO4  when 
boiled  5  minutes.  (Siegle,  J.  pr.  69.  142.) 


938 


SULPHATE,  BARIUM 


Solubility  of  BaSO4  in  HCl+Aq. 


No.  cc. 
HC1  +Aq 
containing 


equi 


1   mg. 
liv.  H 


Cl 


2.0 
1.0 
0.5 
0.2 


Mg.  BaSO4 

per  1  mg. 

equiv.  of 

HC1 


0.133 

0.089 
0.056 
0.017 


g.  per  100  cc.  solution 


HC1 


BaS04 
0.0067 

0.0089 
0.0101 
0.0086 


(Banthisch,  J.  pr.  1884,  29.  54.) 

100,000  pts.  H2O  dissolve  0.124  pt.  BaSO4; 
1000  pts.  HNOs+Aq  of  1.167  sp.  gr.  dissolve 
2  pts.  BaSO4;  1000  pts.  HNO3+Aq  of  1.032 
sp.  gr.  dissolve  0.062  pt.  BaSO4.  (Calvert, 
Chem.  Gaz.  1856.  55.) 

When  0.4  g.  BaSO4  is  heated  K  hour  with 
150  ccm.  HNO3+Aq  of  1.02  sp.  gr.,  0.165  g. 
is  dissolved.  (Siegle,  J.  pr.  69.  142.) 

Solubility  of  BaSO4  in  HNO3+Aq. 


No.  cc. 

HNOs+Aq 

containing 

1  mg.  equiv. 

HN03 


2.0 
1.0 

0.5 
0.2 


Mg.  BaSO4 

per  1  mg. 

equiv.  of 

BaS04 


0.140 
0.107 
0.085 
0.048 


G.  per  100  cc.  solution 


HN03 
3.15 

6.31 
12.61 
31.52 


BaSO4 


0.0070 
0.0107 
0.0170 
0.0241 


(Banthisch,  J.  pr.  1884,  29.  54.) 

Acetic  acid  has  less  solvent  power  than 
other  acids.  80  ccm.  HC2H3O2+Aq  of  1.02 
sp.  gr.  boiled  with  0.4  g.  BaSO4  K  hour  dis- 
solve 0.002  g.  (Siegle,  J.  pr.  69.  142.) 

Sol.  in  boiling  cone.  H2SO4.  (See 
BaH2(S04)2). 

Sol.  in  fuming  H2SO4.    (See  BaS2O7.) 

Sol.  in  2500  pts.  boiling  40%  HBr+Aq;  in 
6000  pts.  boiling  40%  HI+Aq.  (Haslam, 
C.  N.  63.  87.) 

Sol.  in  considerable  amount  in  metaphos- 
phoric  acid+Aq.  (Scheerer  and  Drechsel, 
J.  pr.  (2)  7.  68.) 

Not  attacked  by  boiling  cone.  KOH+Aq  if 
CO2  is  not  present.  (Rose,  Pogg.  95.  104.) 

Very  si.  decomp.  by  standing  a  long  time 
with  cold  cone,  alkali  carbonates +Aq. 

Decomp.  by  boiling  Na2CO3  or  K2CO3+ 
Aq,  not  by  (NH4)2CO3+Aq.  (See  Storer's 
Diet,  for  analytical  data.) 

Very  si.  sol.  in  NH4Cl+Aq,  1  pt.  dissolv- 
ing in  230,000  pts.  sat.  NH4Cl+Aq. 

500  ccm.  sat.  NH4NO3+Aq  with  50  ccm. 
sat.  NH4Cl+Aq  dissolve  2  g.  BaSO4.  100 
ccm.  sat.  NH4NO3+Aq  with  100  ccm.  sat. 
NH4Cl+Aq  dissolve  only  0.08  g.  BaSO4, 
therefore  above  solubility  is  due  to  free 
chlorine.  (Mittentzwey,  J.  pr.  75.  214.) 

BaS04  cannot  be  precipitated  from  solu- 
tions containing  free  C12.  (Erdmann,  J.  pr. 
75.  215.) 


Pptn.  is  retarded  si.  by  tartaric  and  racemic 
acids.  (Spiller.) 

Na  metaphosphate  prevents  pptn.  of  BaSO4 
but  not  ortho-  or  pyrophosphate.  (Scheerer, 
J.  pr.  75.  114.) 

Not  precipitated  in  presence  of  alkali  ci- 
trates. (Spiller.) 

Much  less  sol.  in  NH4Cl+Aq  than  in 
NH4NO3+Aq.  Insol.  in  warm  cone.  Na2S203 
+Aq.  (Diehl,  J.  pr.  79.  431.) 

Not  appreciably  sol.  in  H2O  containing 
ammonium  or  sodium  chloride.  (Brett,  Witt- 
stein,  Wackenroder.) 

Not  appreciably  sol.  in  H2O  at  250°,  or  in 
H2O  containing  Na2S.  (Senarmont.) 

Solubility  is  increased  by  alkali  nitrates, 
but  not  appreciably  by  NaCl,  KC103,  or 
Ba(NO3)2.  (Fresenius,  Z.  anal.  9.  52.) 
Scarcely  sol.  in  boiling  cone.  (NH4)2SO4+Aq. 
(Fresenius.) 

Solubility  in  H2O  increased  by  presence  of 
MgCl2  (Fresenius);  cerium  salts  (Marignac). 

Sol.  in  Fe2Cl6+Aq.  (Lunge,  Z.  anal.  19. 
141.) 

Solubility  in  various  salts +Aq  at  20-25°. 


g.  salt 

Mg.  BaSO4  dissolved  per  1.  in 

per  1. 

FeCh 

A1C13 

MgCh' 

1 

58 

33 

30 

2.5 

72 

43 

30 

5 

115 

60 

33 

10 

123 

9,4 

33 

25 

150 

116 

50 

50 

160 

170 

50 

100 

170 

175 

50 

(Fraps,  Am.  Ch.  J.  1902,  27.  290.) 

Solubility  in  sat.  solution  of  various  salts+ 
Aq. 


Salt 


NaNO3 

NaCl 

NH4C1 


G.  BaSO4  sol.  in  1  1. 
of  the  solvent    , 

0.2940 

0.00783 

0.00827 


(Ehlert,  Z.  Elektrochem,  1912,  18.  728.) 

Cone.  CrCl3+Aq  dissolves  40-120  times 
as  much  BaSO4  as  H2O,  when  boiled  there- 
with for  5  days;  cone.  CrCl3+Aq  acidified 
with  HC1,  450  times  as  much  in  10  days. 
(Kuster,  Z.  anorg.  1905,  43.  348.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Sol.  in  H2O2+Aq.  (Gawalowski,  C.  C. 
1906,  II.  7.) 

100  cc.  95%  formic  acid  dissolve  0.01  g. 
BaSO4  at  18.5°.  (Aschan,  Ch.  Ztg.  1913,  37. 
1117.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790) ;  in  ethyl  acetate.  (Naumann, 
B.  1904,  37.  3601.) 

Min.  Barite. 


SULPHATE,  BISMUTH  POTASSIUM 


939 


Barium  hydrogen  sulphate,  BaH2(SO4)2. 

100  pts.  H2SO4  dissolve  2.22  pts.  BaSO4 
(Lies-Bodart  and  Jacquemin,  C.  R.  46.  1206); 
5.69  pts.  BaSO4  (Struve,  Z.  anal.  9.  34). 

Boiling  H2SO4  dissolves  10-12%  freshly 
precipitated  BaSO4  without  separating  crys- 
tals on  cooling.  H2SO4  at  100°  dissolves 
more  than  boiling  H2SO4,  and  becomes  cloudy 
if  heated  to  boiling.  (Schultz,  Pogg.  133. 
146.) 

1  g.  BaSO4  pptd.  from  BaCl2  is  sol.  in  3153 
g.  91%  H2SO4;  from  Ba(NO3)2  is  sol.  in  1519 
g.  91%  H2SO4.  (Varenne  and  Pauleau,  C.  R. 
93.  1016.) 

100  pts.  hot  cone.  H2SO4  dissolve  approx. 
6  pts.  BaSO4.  (Rohland,  Z.  anorg.  1910,  66. 
206.) 

10  ccm.  of  sat.  BaSCX-f- absolute  H2SO4 
contain  approx.  2.851  g.  BaSO4.  (Bergius, 
Z.  phys.  Ch.  1910,  72.  355.) 

Equilibrium  in  the  system  BaSO4+H2SO4  + 
H2O  at  25°. 


Composition  of  the  solution 


%  H2SC)4 

g.  BaS04 
per  1. 

Solid  phase 

73.83 
78.04 
80.54 
83.10 
85.78 
88.08 
93.17 

0.030 
0.135 
0.285 
0.800 
3.215 
12.200 
49.665 

BaSO4 
ii 

u 
it 

BaS04,  2H2S04.H 

a 

BaSO4,  H2SO4 

20 

(Volkhonski,  C.  C.  1910,  I.  1954;  C.  A.  1911. 

617.) 

Decomp.  by  H2O,  alcohol,  or  ether. 

+2H2O.    (Schultz.) 

BaSO4,  2H2SO4+H2O.    (Volkhonski.) 

Barium  pyrosulphate,  BaS2O7. 

100  pts.  fuming  H2SO4  dissolve  15.89  pts. 
BaSO4.  (Struve,  Z.  anal.  9.  34.) 

Very  deliquescent. 

Decomp.  with  H2O  with  hissing.  (Schultz- 
Sellack,  B.  4.  111.) 

Barium  calcium  sulphate,  3BaSO4,  CaSO4. 
Min.  Dreelite. 

Barium  platinic  sulphate  (?). 

Insol.  in  H2O  or  boiling  HC1  or  HNO3+Aq.  Sol.  in 
hot  cone.  H2SO4  or  aqua  regia.  (E.  Davy.) 

Barium    tin    (stannic)    sulphate,    BaSO4, 

Sn(SO4)2+3H2O. 

Decomp.  by  H2O.  Insol.  in  HC1.  (Wein- 
land  and  Kiihl,  Z.  anorg.  1907,  64.  249.) 

Barium  titanium  sulphate,  2BaSO4,  3Ti(SO4)2. 
Ppt.    Decomp.  byH2O,  giving  titanic  acid. 
(Weinland,  Z.  anorg.  1907,  64.  255.) 


Barium  sulphate  potassium  chloride,  3BaSO4, 

KC1. 
Ppt.    (Silberberger,  M.  1904,  25.  233.) 

Bismuth  sulphate,  basic,  (BiO)2SO4. 

Insol.  in  H2O.  Sol.  in  HNO3  or  H2SO4  + 
Aq. 

+2H2O.    (Heintz,  Pogg.  63.  55.) 

4Bi2O3,  3SO3  +  15H2O.  Insol.  in  H2O. 
(Leist.) 

(BiO)HSO4+H2O.  Insol.  in  H2O.  Sol.  in 
dil.  H2SO4+Aq. 

+2H2O.  Decomp.  by  H2O  with  separation 
of  (BiO)2SO4+2H2O.  (Heintz.) 

3Bi2O3,  2SO3+2H2O.  Insol.  in  H2O. 
(Athanasesco,  C.  R.  103.  271.) 

5Bi2Q3,  11SO3+17H2O.  This  sulphate 
crystallizes  out  from  sulphuric  acid  of  any 
strength  between  H2SO4,  6H2O  and  H2SO4, 
12H2O.  (Adie,  Proc.  Chem.  Soc.  1899,  15. 
226.) 

Bi2O3,  2SO3,  2^H2O  is  in  equilibrium  at 
50°  with  5.4-51.4%  H2SO4-hAq. 

Bi2O3,  SO3  is  in  equilibrium  at  50°  with 
acid  solutions  weaker  than  5.4%  H2SO4. 
(Allan,  Am.  Ch.  J.  1902,  27.  287.) 

• 

Bismuth  sulphate,  Bi2(SO4)3. 

Very  hygroscopic.  Takes  up  H2O  with 
strong  evolution  of  heat  to  form  2Bi2(SO4)3  + 
7H2O,  which  becomes  Bi2(SO4)3+3H2O  at 
100°.  Decomp.  by  boiling  H2O  into  Bi2O3, 
SO3+H2O.  (Hensgen,  J.  B.  1886.  552.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Bismuth  sulphate,  acid,  Bi2O3,  4SO3. 

Bi2O3,  4SO3  is  in  equilibrium  at  50°  with 
51.4-90%  H2SO4+Aq.  (Allan,  Am.  Ch.  J. 
1902,  27.  287.) 

+H2O.  Crystallizes  out  from  sulphuric 
acid  at  temp,  above  170°.  (Adie,  Proc.  Chem. 
Soc.  1899,  16.  226.) 

+3H2O.  Crystallizes  from  sulphuric  acid 
of  any  strength  between  H2SO4,  H2O  and 
H2SO4,  2H2O.  (Adie.) 

+7,  or  9H2O  =  BiH(SO4)2+3H29.  Insol. 
in  H2O.  Easily  sol.  in  acids,  especially  HC1, 
and  HNO3+Aq.  (Leist,  A.  160.  29.) 

+7H2O.  Crystallizes  out  from  sulphuric 
acid  of  any  strength  between  H2SO4,  3H2O 
and  H2SO4,  5H2O. 

+10H2O.  Crystallizes  out  from  sulphuric 
acid  at  temp,  below  170°.  (Adie.) 

Bismuth  potassium  sulphate,  Bi2(SO4)3, 
3K2SO4  (?). 

Decomp.  by  H2O;  insol.  in  sat.  K2SO4+Aq. 
(Heintz.) 

Bi2(SO4)3,  2K2SO4. 

BiK(SO4)2  =  Bi2(SO4)3,  K2SO4.  Insol.  in 
cold  H2O;  decomp.  by  boiling.  (Brigham, 
Am.  Ch.  J.  14.  170.) 


940 


SULPHATE,  BISMUTH  SODIUM 


Bismuth  sodium  sulphate,  Bi4Na6(SO4)9. 

Sp.gr. 

of  CdSO4+Aq  at  18°. 

(Ludecke,  A.  140.  277.) 

%  CdSO 

4                  1 

5 

10 

15 

Boron  sulphate. 

Sp.gr. 

1.0084 

1.0486     1 

.1026 

1.1607 

See  Boro  sulphuric  acid. 

%CdSO 

4      .    20 

25 

30 

35 

Sp.gr. 

1.2245 

1.295       1 

.3725 

1.4575 

Bromomolybdenum  sulphate. 

See  under  Bromomolybdenum  compounds. 

%  CdSO 

4         36 

Sp.  gr. 

1.4743 

Cadmium  sulphate,  basic,  2CdO,  SO3,  and 
+H20. 

Difficultly  sol.  in  H20.  (Stromeyer.)  SI. 
sol.  in  hot  H2O.  (Habermann,  M.  5.  432.) 

4CdO,  SO3.  (Pickering,  Chem.  Soc.  1907, 
91.  1987.) 

Cadmium  sulphate,  CdSO4. 
Sat.  CdSO4+Aq  contains  at: 
0°          10°        24°        30°        65° 
35.9       37.5       41.5       42.0       49.7%  CdSO4, 

86°      94°     130°     165°    188°    200° 
43.5    91.6    27.7     14.7      7.1      2.3%  CdSO4. 
CdSO4    easily    forms    supersat.    solutions, 
(fitard,  A.  ch.  1894,  (7)  2.  552.) 

Solubility  in  H2O. 


t° 

Per  cent  CdSO4 
in  sat.  solution 

Solid  phase 

-18 

43.35 

Ice 

-10 

43.27 

u 

0 

43.01 

CdS04,  8/sH20 

+10 

43.18 

15 

43.20 

20 

43.37 

30 

43.75 

40 

43.99 

60 

44.99 

62 

45.06 

72 

46.2 

73.5 

46.6 

74.5 

46.7 

75 

46.5 

CdSO 

,H20 

77 

42.2 

78.5 

41.5 

85 

39.6 

90 

38.7 

95 

38.1 

100 

37.8 

H 

(Mylius  and  Funk,  B.   1897,  30.  825.) 
See  also  under  CdSO4+22/3H2O,  and  7H2O. 

Sp.  gr.  at  0°/4°  of  CdSO4-f  Aq  containing 
14.0  g.  CdS04  in  1000  g.  H2O  =  1.0122. 

Sp.  gr.  at  12°/4°  of  CdSO4+Aq  containing 
14.0  g.  CdSO4  in  100  g.  H2O  =  1.0121. 

Sp.  gr.  at  1274°  of  CdSO4+Aq  containing 
57.2  g.  CdSO4  in  1000  g.  H20  =  1.0514. 

Sp.  gr.  at  0740  of  CdSO4+Aq  containing 
183.1  g.  CdSO4  in  1000  g.  H2O  =  1.1552. 

Sp.  gr.  at  1374°  of  CdSO4+Aq  containing 
183.1  g.  CdSO4  in  1000  g.  H2O  =  1.1529. 
(Fouque",  Ann.  Observ.  1868,  9.  172.) 


(Grotrian,  W.  Ann.  1883,  18.  193.) 

Sp.  gr.  of  CdSO4+Aq  at  room  temp,  con- 
taining: 

7.14         14.66       22.011%  CdSO4. 
1.0681       1.1591         1.2681 

(Wagner,  W.  Ann.  1883,  18.  268.) 
Sp.  gr.  of  CdSO4+Aq  at  25°. 


Concentration  of  CdSCh 
+Aq 

Sp.  gr. 

1-normal 

Vr-       " 

V<~          " 

Vr-       " 

1.0973 
1.0487 
1.0244 
1.0120 

(Wagner,  Z.  phys.  Ch.  1890,  5.  36.) 
Sp.  gr.  of  CdSO4+Aq. 


%  CdS04 

t 

Sp.  gr.  at  t° 

Sp.  gr.  at  18° 

0.0289 

0^0498 
0.0999 
0.495 
0.981 

17.29 
23.65 
18.00 
18.00 
18.00 
18.00 

0.99908 
0.99776 

0.99893 

0.99915 
0.99961 
1.0034 

1.0084 

(Wershofen,    Z.    phys.    Ch.    1890,    5.    494.) 

Sp.  gr.  at  16°/4°  of  CdSO4+Aq  containing 
29.4654%  CdSO4  =  1.36289;  containing 
21.3671%  CdSO4  =  1.24211.  (Schonrock,  Z. 
phys.  Ch.  1893,  11.  781.) 

Sp.  gr.  of  CdSO4+Aq  at  18°/4°. 

%  CdSO4       25.121  18.172 

Sp.  gr.  1.297  1.200 


%  CdS04 
Sp.  gr. 

(de  Muynck,  W.  Ann.  1894,  53.  561.) 


9.952 
1.101 


5.639 
1.055 


CdSO4+Aq  containing  13.40%  CdSO4  has 
sp.  gr.  20°/20°  =  1.1429. 

CdSO4+Aq  contaiing  16.79%  CdSO4  has 
sp.  gr.  20720°  =  1.1847. 

(Le  Blanc  and  Rohland,  Z.  phys.  Ch.  1896, 
19.  282.) 


SULPHATE,  CADMIUM  OESIUM 


941 


Sp.  gr.  of  CdS04  at  18. 2°,  when  p'=per  cent 
strength  of  solution;  d  =  observed  den- 
sity; w  =  volume  cone,  in  grams  per 


ioo 


p 

d 

w 

39.86 

1.5639 

0.6231 

31.53 

1.4080 

0.4439 

26.85 

1.3310 

0.3574 

24.17 

1.2901 

0.3118 

18.35 

1.2084 

0.2217 

13.27 

1  .  1437 

0.1518 

9.97 

1  .  1045 

0.1102 

7.46 

1.0764 

0.0803 

6.12 

0.0619 

0.0650 

2.52 

0.0242 

0.0259 

1.45 

0.0132 

0.0147 

0.464 

0.0033 

0.0046 

(Barnes,  J.  phys.  Ch.  1898,  2.  543.) 


Sp.  gr.  of  CdSO4+Aq  sat.  at  25°  and  1  atm. 
=  1.617.  (Sinnige,  Z.  phys.  Ch.  1909,  67. 
518.) 

See  also  under  CdSO4+22/3H2O,  and 
+4H20. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329);  methyl  acetate.  (Naumann,  B.  1909, 
42.  3790);  ethyl  acetate:  (Naumann,  B. 
1910,  43.  314.) 

+H2O.  See  Mylius  and  Funk,  under 
CdSO4. 

•flVi  H2O.  (Worobieff,  Bull.  Soc.  1896, 
(3)  16.  1754.) 

+22/3H2O.  1  pt.  H2O  dissolves  0.59  pt. 
anhydrous  salt  at  23°,  and  not  much  more  on 
heating.  Sat.  solution  boils  at  102°.  Pre- 
cipitated by  alcohol,  (v.  Hauer.) 


100  g.  H2O  dissolve  g.  CdSO4  at  tc 


100  pts.  H2O  dissolves  at: 
13.7°   14.98°  15.0°  16.0° 
76.06  76.09    76.14  76.18  pts.  anhydrous  salt, 

16.96°  18.0°   19.0°  25.0° 
76.26    76.32  76.39  76.81  pts.  anhydrous  salt. 
(Steinwehr,  W.  Ann.  1902,  (4)  9.  1050.) 

100  g.  H2O  dissolve  76.02  g.  CdSO4  at  25°. 
(Stortenbecker,  Z.  phys.  Ch.  1900,  34.  109.) 

Solubility    of   CdSO4+22/3H2O    at    25°    and 
varying  pressures. 


Pressure  in  atmospheres 

G.  CdSO4  in  100  g.  H2O 

1 

500     .  ., 
500 
1000 
1000 

76.80 

77.85 
78.08 

78.77 
78.68 

Det.  by  another  method 


Pressure  in  atmospheres 

G.  CdS04  inlOO  g.  H2O 

250 
500 
750 
1000 

77.53 
78.02 
78.60 
78.96 

(Cohen  and  Sinnige,  Trans.  Farad.  Soc.  1910, 
6.  269.) 

Sp.  gr.  at  21.6°/0°  of  CdSO4+Aq  contain- 
ing 11.47%  CdSO4+8/3H2O  =  1.0944.  (Ka- 
nonnikoff,  J.  pr.  1885,  (2)  31.  346.) 

100  g.  H2O  dissolve  57.61  g.  CdSO4+ 
10.63  g.  FeSO4  at  25°.  (Stortenbecker,  Z. 
phys.  Ch.  1900,  34.  109.) 

+4H2O.  (Lescoeur,  A.  ch.  1895,  (7)  4. 
222.)' 

Sp.  gr.  at  15°  of  CdSO4+Aq  containing 
10  g.  CdSO4+4H2O  in  100  c.c  of  solution  = 
1.0790;  containing  20  g.  CdSO4+4H2O  in 
100  cc.  of  solution  =  1.1 522.  (Traube,  J.  pr. 
1885,  (2)  31.  207.) 

Could  not  be  obtained.  (Mvlius  and 
Funk.) 

+7H20. 

Solubility  in  H2O. 


t° 

G.  CdS04 

t° 

%  CdS04 

0 
5 
7 
9 
11.5 
13 
15 
16 
17 
18 
19 
25 

75.52 
75.65 
65.73 
75.85 
75.94 
76.04 
76.11 
76.16 
76.13 
76.14 
76.18 
76.79 

-17 

-16 
-12 
-10 

-  7 
-  5 
-  4.5 

44.45 
44.5 
45.3 
46.1 
47.5 
48.5 
48.7 

(Mylius  and  Funk,  B.  1897,  30.  828.) 

Cadmium  caesium  sulphate,  CdSO4,  Cs2SO4-f 
6H20. 
Sol.  in  H2O.    (Tutton,  Chem.  Soc.  63.  337.) 
1    1.    H2O   dissolves   1399    g.    anhydrous 
salt  at  25°.    (Locke,  Am.  Ch.  J.  1902,  27.  459.) 

(Kohnstamm  and  Cohen,  W.  Ann.  1898,  65. 
352.) 

942 


SULPHATE,  CADMIUM  CALCIUM  POTASSIUM 


Cadmium  calcium  potassium  sulphate, 

Ca2CdK2(SO4)4+2H2O. 
(D'Ans,  B.  1908,  41.  1778.) 

Cadmium  cerium  sulphate,  CdSO4,  Ce2(SO4)3 
+6H2O. 
Sol.inH2O.    (Wyrouboff.) 

Cadmium  hydrazine  sulphate, 

Solubility  of  CdNa2(SO4)2,  2H2O+CdSO4, 
8/3  H2O  in  100  g.  H2O  at  t°. 

t° 

0 
5 
10 

V,     •» 

go 

Sco 

2-T3 

00 

73.54 
73.38 

72.765 

See 

c£ 

8.85 
8  .  67.r: 
9.55 

t 

15 

20 
25 

|o 

00 

73  .  76" 
73  .  81 
73.71 

II 

t° 

SO 

00 

Ji- 

9.. 435 
9.455 
10.48 

30 
35 
40 

73.915 
75.01 
75  .  385 

ll.  10 
12   32 
13'75 

CdH2(SO4)2,  2N2H4. 

1  pt.  is  sol.  in  202.5  pts.  H2O  at  12°. 

Not  attacked  by  dil.  acids.  Easily  sol.  in 
NH4OH+Aq.  (Curtius,  J.  pr.  1894,  (2)  50. 
331.) 

Cadmium    magnesium    sulphate,    CdSO4, 

MgSO4+14H2O. 

Very  efflorescent.  Sol.  in  H2O.  (Schiff,  A. 
104.  325.) 

Cadmium  potassium  sulphate,  K2SO4,  CdSO4 


Sol.  in  H2O.     (v.  Hauer,  Pogg.  133.  176.) 

100  pts.  H2O  dissolve  42.50  pts.  anhydrous 
salt  at  26°; 

100  pts.  H2O  dissolves  42.80  pts.  anhydrous 
salt  at  31°; 

100  pts.  H2O  dissolve  43.45  pts.  any  hydrous 
salt  at  40°; 

100  pts.  H2O  dissolve  44.90  pts.  anyhydrous 
salt  at  64°.  (Wyrouboff,  Bull.  Soc.  Min. 
1901,  24.  68.) 

+2H2O.  100  pts.  H2O  dissolve  42.89  pts. 
anhydrous  salt  at  16°;  46.82  pts.  at  31°; 
47.40  pts.  at  40°.  (Wyrouboff.) 

+4H2O.  Efflorescent.  (Wyrouboff,  Bull. 
Soc.  Min.  1891,  14.  235.)  .A 

+6H2O.  Very  efflorescent,  and  easily 
decomp.  (Schiff.) 

Does  not  exist.     (Wyrouboff.) 

Cadmium    rubidium    sulphate,    CdSO4, 

Rb2S04+6H2O. 

Efflorescent.      Sol.    in    H2O.      (Tutton.) 
1  1.  H2O  dissolves  767  g.  anhydrous  salt 

at  25°.     (Locke,  Am.  Ch.  J.  1902,  27.  459.) 

Cadmium  sodium  sulphate,  CdSO4,  Na2SO4  + 

2H2O. 
Sol.  in  H2O.    (v.  Hauer.) 

Solubility  of  CdNa2(SO4)2+2H2O  in  100  g. 
H2O  at  t°. 


t° 

Grams  CdSO4 

Grams  Na2SO4 

24 

35.49 

24.04 

25 

35.88 

24.46 

30 

36.28 

24.605 

35 

36.69 

24.99 

40 

37.24 

25.455 

(Koppel,  Z.  phys.  Ch.  1905,  52.  413.) 
Decomp.  by  H2O  below  20.5°. 


(Koppel.) 

Solubility   of    CdNa2(SO4)2,  2H2O+Na2SO4, 
10H2O  in  100  g.  H2O  at  t°. 


t° 

Grams  CdSO4 

Grams  NazSCU 

-14.8 

72.68 

8.32 

0 

66.325 

11.625 

5 

61.78 

12.97 

10 

55.34 

14.785 

12 

51.615 

15.95 

15 

46.60 

17.99 

19.8 

36.13 

22.16 

20 

36.25 

23.52 

24 

27.82 

29.17 

25 

25.59 

31.08 

30 

14.62 

44.145 

(Koppel.) 

Solubility    of    CdNa2(SO4)2,    2H2O+Na2SO4 
(anhydrous)  in  100  g.  H2O  at  t°. 


t° 

Grams  CdSCh 

Grams  Na2SC>4 

35 
40 

13.26 
16.25 

47.06 
46.27 

(Koppel.) 

Cadmium  sulphate  ammonia,  CdSO4,  6NH3. 

Sol.  in  H2O  with  separation  of  CdO.  (Rose, 
Pogg.  20.  152.) 

CdSO4,  4NH3+4H2O.  Decomp.  by  H2O. 
(Malaguti  and  Sarzeau,  A.  ch.  (3)  9.  431.) 

+2H2O.     Ppt.     (Andre,  C.  R.  104.  987.) 

+2^H2O.  Sol.  in  H2O  with  separation  of 
basic  sulphate.  (Mttller,  A.  149.  70.) 

CdSO4,  3NH3.  (Isambert,  C.  R.  1870,  70. 
457.) 

Cadmium  sulphate  cupric  oxide,  CdSO4, 
3CuO+zH2O. 

(Recoura,  C.  R.  1901,  132.1415.) 

2CdSO4,  3CuO+8H2O.  (Mailhe,  A.  ch. 
1902,  (7)  27.  383.) 

+  12H2O.     (Mailhe.) 

6CdSO4,  20CuO+rcH2O.  fRecoura,  C.  R. 
1901,  132.  1415.) 

Cadmium      sulphate      hydrazine,      CdSO4, 

2N2H4. 

Easily  sol.  in  NH4OH+Aq  but  cannot  be 
cryst.  therefrom.  (Franzen,  Z.  anorg.  1908, 
60.  282.) 


SULPHATE,  CAESIUM  IRON 


943 


Cadmium   sulphate  hydrogen   chloride, 
3CdSO4,  4HC1+4H2O. 
Very  deliquescent.    (Baskerville  and  Harris, 
J.  Am.  Chem.  Soc.  1901,  23.  896.) 
3CdS04,  8HC1.    Very  deliquescent.    (Bas- 
kerville and  Harris.) 

Caesium  sulphate,  Cs2SO4. 

Solubility  in  H2O. 

Temp. 

G.  per  litre 

G.  mols. 
anhydrous 
salt  per  1. 

25° 
30° 
35° 
40° 

5.7 
9.6 

12.06 
15.3 

0.015 
0.025 
0.032 
0.0405 

100  pts.  H2O  dissolve  158.7  pts.  Cs2SO4  at 
—2°. 

100  cc.  H2O  at  17-18°  dissolve  163.5  g. 
Cs2SO4.  (Tutton,  Chem.  Soc.  1894,  65. 
632.) 

Solubility  in  H2O. 


G.  Cs2S04 

G.  Cs2SO4 

*° 

per  100  g. 

•io- 

t° 

per  100  g. 

150- 

Solu- 
tion 

H2O 

3$ 

Solu- 
tion 

H2O 

d^ 

0 

62.6 

167.1 

3.42 

60 

66.7 

199.9 

3.78 

10 

63.4 

173.1 

3.49 

70 

67.2 

205.0 

3.83 

20 

64.1 

178.7 

3.56 

80 

67.8 

210.3 

3.88 

30 

64.8 

184.1 

3.62 

90 

68.3 

214.9 

3.92 

40 

65.5 

189.9 

3.68 

100 

68.8 

220.3 

3.97 

5,0 

66.1 

194.9 

3.73 

108.6 

69.2 

224.5 

4.00 

(Berkeley,  Trans.  Roy.   Soc.   1904,   203.   A. 
210.) 

Solubility  in  Na2SO4+Aq. 

Sat.  solution  contains  54.7%  Cs2SO4+ 
11.45%  Na2SO4  at  25°.  (Foote,  J.  Am. 
Chem.  Soc.  1911,  33.  467.) 

Insol.  in  alcohol.     (Bunsen.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329);  (Eidmann,  C.  C.  1899,  II.  1014.) 

Solubility  in  glycol  at  ord.  temp.  =  3.0- 
3.2%.  (de  Coninck,  Belg.  Acad.  Bull. 
1905.  359.) 

Caesium  hydrogen  sulphate,  CsHSO4. 
Sol.  in  H2O. 

Caesium  pyrosulpha.te,  Cs2S2O7. 
Decomp.  by  H2O. 

Caesium  ocfosulphate,  Cs2S8O25. 

Decomp.  by  H2O.     (Weber,  B.  17.  2497.) 

Caesium  calcium  sulphate,  Ca2Cs2(S04)3. 
Very  stable,     (D-'Ans,  B.  1908,  41.  1776.) 

Caesium    chromium    sulphate,    Cs2Cr2(SO4)4 

+24H20. 
Melts  in  crystal  H2O  at  116°.     (Locke.) 


(Locke,  Am.  Ch.  J.  1901,  26.  180.) 


Caesium  cobaltous  sulphate,  Cs2S04,  CoSO4-j- 
6H20. 

Sol.  in  H2O.  (Tutton,  Chem.  Soc.  63. 
337.) 

1  1.  H2O  dissolves  418.8  g.  anhydrous 
salt  at  25°.  (Locke,  Am.  Ch.  J.  1902,  27. 
459.) 

Caesium    cobaltic    sulphate,    Cs2Co2(SO4)4+ 

24H20. 

Melts  in  crystal  H2O  at  116°.  (Locke, 
Am.  Ch.  J.  1901,  26.  183.) 

Caesium  copper  sulphate,  Cs2SO4,  CuSO4  + 
6H2O. 

Sol.  in  H2O.    (Tutton.) 

1  1.  H2O  dissolves  460  g.  anhydrous  salt 
at  25°.  (Locke,  Am.  Ch.  J.  1902,  27.  459.) 

Caesium   gallium    sulphate,    Cs2Ga2(SO4)4+ 

24H2O. 

(Soret,  Arch.  sc.  phys.  nat.  1888,  (3)  20. 
531.) 

Caesium  indium  sulphate,  Cs2In2(SO4)4+ 
24H2O. 

75.7  g.  anhydrous  (117.39  hydrated)  salt 
or  0.172  g.  mols  of  anhydrous  salt  are  sol. 
in  1  1.  H2O  at  25°.  (Locke,  Am.  Ch.  J.  1901, 
26.  175.) 

100  pts.  H2O  dissolve  3.04  pts.  at  16.5°. 
(Chabrie  and  Rengade,  C.  R.  1900, 131. 1301.) 

Caesium  indium  sulphate,  Cs2SO4, 
Ir2(S04)3+24H20. 

Mpt.  109-110.° 

Very  si.  sol.  in  cold.  More  easily  sol.  in 
hot  H2O.  (Marino,  Z.  anorg.  1904,  42.  218.) 

Caesium  iron  (ferrous)  sulphate.  Cs2SO4. 
FeSO4+6H2O. 

Sol.  in  H2O.     (Tutton.) 

1  1.  H2O  dissolves  1011  g.  anhydrous  salt 
at  25°.  (Locke,  Am.  Ch.  J.  1902,  27.  459.) 

Caesium  iron  (ferric)  sulphate,  Cs2Fe2(SO4)4 
+24H2O. 

Melts  in  crystal  H2O  at  71°.     (Locke.) 


944 


SULPHATE,  CESIUM  LANTHANUM 


Solubility  in  H2O. 

Caesium      thallic     sulphate,      CsTl(SO4)4-f 
13^H2O. 

Hygroscopic.     (Locke,  Am.  Ch.  J.   1902, 
27.  283.) 
+3H2O.     Very  si.  sol.  in  cold;  easily  sol. 
in  hot  H2O.    Can  be  recryst.  from  H2SO4-j- 
Aq.    The  recryst.  salt  is  at  once  decomp.  by 
H2O  or  95%  alcohol.    (Locke.) 

t° 

G.  per  litre 

G.  mols. 
anhydrous  salt 
per  litre 

25 
30 
35 
40 

17.1 
25.2 
37.5 
60.4 

0.045 
0.066 
0.099 
0.156 

(Locke,  Am.  Ch.  J.  1901,  26.  180.) 

Caesium  lanthanum  sulphate,  Cs2SO4, 
La2(SO4)3+2H2O. 

(Baskerville,  J.  Am.  Chem.  Soc.  1904, 
26.^67.) 

2Cs2SO4,  3La2(SO4)3.    (Baskerville.) 

Caesium  magnesium  sulphate,  Cs2SO4, 
MgSO4+6H2O. 

Sol.  in  H2O.     (Tutton.) 

1  1.  H2O  dissolves  533  g.  anhydrous  salt 
at  25°.  (Locke,  Am.  Ch.  J.  1902,  27.  459.) 

Caesium  manganous  sulphate,  Cs2S04, 
MnSO4+8H2O. 

Sol.  in  H2O.    (Tutton.) 

Sol.  in  H2O  and  acids  with  decomp.  (Pic- 
cini,  Z.  anorg.  1899,  20.  14.) 

1  1.  H2O  dissolves  804  g.  anhydrous  salt 
at  25°.  (Locke,  Am.  Ch.  J.  1902,  27.  45. 

Caesium  manganic  sulphate,  Cs2SO4, 

Mn2(SO4)3+24H2O. 

Decomp.  by  H2O  and  dil.  acids  with  sep- 
aration of  MnO2.  Sol.  in  1 :3  H2SO4+Aq  and 
in  cone.  HNO3.  Insol.  in  acetic  acid.  Sol. 
in  oxalic  acid+Aq.  (Christensen,  Z.  anorg. 
1901,  27.  332.) 

Caesium     neodymium      sulphate,      Cs2SO4, 

Nd2(SO4)3+3H2O. 

(BaskervUle,  J.  Am.  Chem.  Soc.  1904,  26. 
74.) 

Caesium  nickel   sulphate,   Cs2SO4,   NiSO4  + 

6H20. 

Sol.  in  H2O.    (Tutton.) 
1  1.  H2O  dissolves  255.8  g.  anhydrous  salt 
at  25°.    (Locke,  Am.  Ch.  J.  1902,  27.  459.) 

Caesium  praseodymium  sulphate,  Cs2SO4, 
Pr2(S04)3+2H20. 

(Baskerville,  J.  Am.  Chem.  Soc.  1904,  26. 
73.) 

+4H2O.    (Baskerville.) 

Caesium  rhodium  sulphate,  Cs2SO4,Rh2(SO4)3 

+24H2O. 

SI.  sol.  in  cold,  sol.  in  warm  H2O;  mpt. 
110-111.°  (Piccini,  Z.  anorg.  1901,  27.  64.) 


Caesium  thorium  sulphate,  Cs2SO4,Th(SO4)2-f- 
2H2O. 

SI.  sol.  in  H2O.      (Manuelli,  Gazz.  ch.  it. 
1903,  32.  (2)  523.) 


Caesium  titanium  sulphate,  Cs2SO4,Ti2(SO4)3 
+24H2O. 

Deliquesces  in  the  air  and  is  decomp. 

SI.  sol.  in  cold  H2O;  decomp.  by  hot  H2O. 
(Piccini  Gazz.  ch.  it.  1895,  25.  542.) 

SI.  sol.  in  cold  H2O,  more  sol.  in  hot  H2O 
acidified  with  H2SO4. 

Decomp.  in  neutral  aq.  solution.  (Piccini, 
Z.  anorg.  1898,  17.  356.) 


Caesium  uranyl  sulphate,   Cs2(UO2)(S04)2  + 
2H2O. 

As  Na  salt,     (de  Coninck,   C.   C.   1905, 
1. 1306.) 


Caesium  vanadium  sulphate,  Cs2V2(SO4)4+ 
24H2O. 

7.71  g.  anhydrous  (13.1  g.  hydrated)  salt, 
or  0.0204  gr.  mols.  of  the  anhydrous  salt  are 
sol.  in  1  1.  H2O  at  25°.  (Locke,  Am.  Ch.  J. 
1901,  26.  175.) 

SI.  sol.  in  cold,  easily  sol.  in  hot  H2O.  (Pic- 
cini, Z.  anorg.  1896,  11.  114.) 

100  pts.  H2O  dissolve  0.464  pts.  of  the  salt 
at  10°  and  sp.  gr.  of  the  solution  at  4°/20°  = 
2.033.  More  sol.  in  hot  H2O  than  in  cold. 
[Piccini,  Z.  anorg.  1897,  13.  446.) 


Caesium  zinc  sulphate,  Cs2S04,  ZnS04-f- 
6H2O. 

Sol.  in  H2O.  (Bunsen  and  Kopp,  Pogg. 
113.  337.) 

1  1.  H2O  dissolves  386.3  g.  anhydrous 
salt  at  25°.  (Locke.  Am.  Ch.  J.  1902,  27. 
459.) 

Caesium  zirconium  sulphate,  Zr2O3,(CsSO4)2 

+HH2O. 
Ppt.     (Rosenheim,  B.  1905,  38.  815.) 

alcium  sulphate,  CaSO4,  and  +2H2O. 

The  older  determinations  of  the  solubility 

of  CaSO4  in  H2O  have  little,  but  historical, 

alue,  as  the  solutions  were  usually  either 

non-saturated  or  supersaturated.    They  may 

)e  tabulated  as  follows. 


SULPHATE,  CALCIUM 


945 


A=pts.  H2O    required   for   dissolving    1    pt. 
CaSO4,  and  B  for  1  pt.  CaSO4+2H2O  at  t°. 


t 

A 

B 

Authority 

Hot  or  cold 

500 

Fourcroy 

Cold 

500 

Bergmann 

Boiling 

450 

" 

All  temp. 

322 

Lassaigne 

(?) 

438 

Anthon 

(?) 

250-300 

Dumas 

Hot  or  cold 

578.5 

461^5 

Bucholz 

Cold 

480 

380 

Giese 

Hot 

491 

388 

it 

15-20° 

492 

388 

Tipp 

12.5° 

503 

397 

Lecoq 

100  pts.  H2O  at  t°  dissolve  pts.  CaSO4 


t 

Pts. 
CaS04 

t° 

Pts. 
CaSCU 

t° 

Pts. 
CaSCU 

0 

0.205 

35 

0.254 

70 

0.244 

5 

0.219 

40 

0.252 

80 

0.239 

12 

0.233 

•50 

0.251 

90 

0.231 

20 

0.241 

60 

0.248 

100 

0.217 

30 

0.249 

(Poggiale,  A.  ch.  (3)  8.  469.) 

Poggiale  worked  with  supersat.  solutions. 
(Droeze,  B.  10.  330.) 

H2O  dissolves  CaSO4  most  abundantly  at 
35°  (Poggiale);  at  32-41°  (Marignac). 

1  pt.  CaSO4+2H2O  dissolves  at: 
0°        18°       24°       32°        38° 
in  415       386       378       371       368  pts.  H2O, 

53°       72° 
375       391 

or  (by  calculation) 
dissolves  at: 

0°        18°       24° 
in  525      488       479 

53°       72° 


41° 
in  370 


99° 

451  pts.  H2O, 

pt.  anhydrous  CaSO4 


86° 
417 


41° 
in  468 


474        495 


32° 

470 

86° 
528 


38° 

466  pts.  H2O, 

99° 
571pts.H2O. 


The  above  nonsat.  solutions  are  obtained  by 
using  a  large  excess  of  CaSO4+2H2O.  The 
undissolved  part  retains  its  water  of  crystal- 
lisation. CaSO4,  dehydrated  at  130-140°, 
forms  a  supersaturated  solution  with  H2O  in 
10  minutes,  containing  1  pt.  CaSO4  to  110  pts. 
H2O,  whicn  soon  deposits  crystals.  The  un- 
dissolved part  takes  up  its  water  of  crystal- 
lisation. Ignited  CaSO4  dissolves  very  slowly 
in  H2O,  so  that  in  24  hours  the  solution  con- 
tains Vf  33  to  Vsgs  anhydrous  CaSO4.  By  longer 
contact  solution  continues  with  formation  of 
supersaturated  solutions,  which  contain  after 
10-30  days  Vs72  to  Y«2s  CaSO4,  but  these  be- 
come normal  as  the  anhydrous  CaSO4  gradually 
takes  up  its  water  of  crystallisation.  The 
mineral  anhydrite  behaves  similarly,  water 
taking  up  Yes*  CaSO4  in  1  day,  Vasi  in  40  days, 
and  V457  in  8  months. 

Supersaturated  solutions  are  also  obtained 


by  evaporation  of  a  saturated  solution.  By 
evaporation  with  heat,  solutions  are  obtained 
containing  Ysoe  CaSO4,  and  in  the  cold  with 
Yif2  CaSO4j  in  the  solution  over  the  separated 
CaSO4+2H2O.  Neutralising  dil.  H2SO4+Aq 
with  CaCOa  gives  a  solution  containing  Yin 
CaSO4,  which  crystallises  out  partly  in  24 
hours,  leaving  Y3isCaSp4  dissolved. 

Supersaturated  solutions  containing  Yno  to 
Yiso  CaSO4  deposit  crystals  rapidly;  those 
under  Ysso  do  not  crystallise  spontaneously. 
A  solution  containing  l/zss  shows  crystals  in  14 
days,  and  contains  Ysia  in  1  month, Y«4  in  2 
months,  Y446  in  3  months,  in  spite  of  repeated 
shaking- 
Boiling  diminishes  the  supersaturation 
without  however  removing  it  entirely.  (Mar- 
ignac, A.  ch.  (5)  1.  274.) 

1-  pt.  CaSO4+2H2O  is  sol.  in  443  pts.  H2O 
at  13.7°;  in  447  pts.  H2O  at  14.2°;  in  421  pts. 
H2O  at  20.2°;  in  419  pts.  H2O  at  21.2°;  ind  in 
445  pts.  H2CO3+Aq  sat.  at  18.7°.  (Church, 
J.  B.  1867.  192.) 

Church's  solutions  were  not  sat.  (Droeze, 
B.  10.  330.) 

1000  pts.  H2O  dissolve  2.19  pts.  CaSO4+ 
2H2O  at  16.5°;  2.352  pts.  CaSO4+2H2O  at 
22°.  (Cossa,  Gazz.  ch.  it.  1873.  135.) 

Cossa's  solutions  were  not  saturated. 
(Droeze.) 

CaSO4+2  H2O  is  sol.  in  415  pts.  H2O  at  0°; 
in  412  pts.  H2O  at  5°;  in  407  pts.  H2O  at  10°; 
in  398  pts.  H2O  at  15°;  in  371  pts.  H2O  at  20°; 
in  365  pts.  H2O  at  25°;  in  361  pts.  H2O  at  30°; 
in  359  pts.  H2O  at  35°.  (Droeze,  B.  10.  330.) 

Sol.  in  500  pts.  H20  at  12.5°.  (From  Marig- 
nac's  and  his  own  results,  de  Boisbaudran,  A. 
ch.  (5)  3.  477.) 

CaSO4  is  sol.  in  564.5  pts.  H2O  at  0.8°; 
506.27  pts.  at  14°;  472-3  pts.  at  32.5-38.8°; 
498.73  pts.  at  64°;  533.92  pts.  at  79.6°. 
(Raupenstrauch,  M.  6.  563.) 

According  to  Goldammer  (C.  C.  1888.  708) 
H2O  is  fully  saturated  with  CaSO4  by  shaking 
the  finely-powdered  substance  5  minutes 
therewith. 

The  following  results  were  obtained.  Fig- 
ures denote  pts.  H2O  in  which  1  pt.  CaSO4  was 
dissolved  at  t°  (a)  from  pptd.  CaSO4  "ipse 
fact.,"  (b)  from  pptd.  CaSO4  "gehe,"  (c)  from 
"glacies  mariae  puly.,"  (d)  from  "glacies 
Mariae  pulv./'  containing  less  than  2H2O. 


t° 

a 

b 

c 

t° 

d 

0 
7.5 
15 
22  5 

561.5 
526 
497.5 
481 

558 
526 
497.5 
481.5 

557.5 
520 
493 
479 

0 
'20 

476.5 
436' 

30 
37.5 
45 
60 
75 
90 
100 

475 
463 
473.5 
484 
507.5 
533.5 
556 

475 
469 
474.5 
486.5 
508 
530 
557 

470 
465.5 
470.5 
482 
503 
534 
534.5 

'40 

'60 

80 

100 

450  ' 

476* 
502.5 

547* 

946 


SULPHATE,  CALCIUM 


Burnt  gypsum  easily  forms  supersat.  solu- 
tions containing  nearly  1%  CaSO."  It  forms 
supersat.  solutions  more  readily  at  0°,  and 
that  tendency  decreases  with  increase  of 
temp.,  hence  figures  in  (d)  which  contained 
burnt  gypsum.  (Goldammer.  C.  C.  1888. 
708.) 

Calculated  from  electrical  conductivity  of 
CaSO4+Aq,  1  1.  H2O  dissolves  2.07  g.  CaSO4 
at  18°.  (Kohlrausch  and  Rose,  Z.  phvs.  Ch. 
12.  241.) 

The  anhydrous  salt  varies  in  solubility. 
Solubility  depends  (1)  upon  temp,  and  time 
of  drying,  (2)  upon  the  relative  amount  of 
salt,  (3)  upon  time  of  shaking.  Possibly  a 
and  £  modifications.  (Potilizin,  C.  C.  1894, 
II.  515.) 

2.04  gr.  are  dissolved  in  1  liter  of  sat.  solu- 
tion at  20°.  (Bottger,  Z.  phys.  Ch.  1903, 
46.  603.) 

At  15°  and  after  5  minutes  shaking,  the 
highest  degree  of  supersaturation  which  can 
be  obtained  with  pure  sol.  calcium  sulphate  = 
9.47  g.  of  the  anhydrous  salt  or  11.976  g. 
CaSO4+2H2O  in  1  1.  of  H2O.  (Cavazzi, 
C.  C.  1905, 1.  1694.) 

Solubility  of  CaSO4  in  100  pts.  H2O  at  high 
temp. 


t° 

Pts. 
CaSO4 

t° 

Pts. 
CaS04 

t 

Pts. 
CaS04 

140 
165 

0.078 
0.056 

175-185 
240 

0.027 
0.018 

250 

0.016 

(Tilden  and  Shenstone,  Phil.  Trans.  1884.  31.) 

Pptn.  of  CaSO4  which  has  been  started  by 
heating  solution  to  140-150°  continues  even 
after  solution  has  cooled.  (Storer.) 

CaSO4  is  completely  insol.  in  sea  water  or 
pure  H2O  at  temperatures  between  140°  and 
150.°  (Couste".) 

Solubility  of  CaSO4  in  sea  water  at  tempera- 
tures over  100°.  t°  =  temp. ;  P  =  pressure 
in  atmospheres;  %=per  cent  CaSO4  in 
sat.  solution. 


t° 

p 

% 

t° 

p 

% 

103 

1 

0.500 

118.5 

1.50 

0.226 

103.8 

1 

0.477 

121.2 

1.5 

0.183 

105.15 

1 

0.432 

124 

2 

0.140 

108.6 

1.25 

0.395 

127.9 

2 

0.097 

111 

1.25 

0.355 

130  ° 

2.5 

0.060 

113.2 

1.25 

0.310 

133.3 

2.5 

0.023 

115.8 

1.50 

0.267 

(Couste',  Ann.  Min.  (5)  6.  80.) 

Solubility  of  CaSO4  in  H2O  at  various  pres- 
sures. 

100  g.  sat.  CaSO4+Aq  at  1  atmos.  pressure 
and  15°  contain  0.206  g.  CaSO4;  at  20  atmos. 
pressure  and  15°  contain  0.227  g.  CaSO4;  at 
1  atmos.  pressure  and  16.2°  contain  0.213  g. 
CaSO4.  (Moller,  Pogg.  117.  386.) 


Soluble  anhydrite: 

1  1.  H2O  dissolves  22.8  milliequivalents  at 
100°. 

1  1.  H2O  dissolves  6.4  milliequivalents  at 
156.° 

Anhydrite: 

1  1.  H2O  dissolves  9.2  milliequivalents  at 
100°. 

1  1.  H2O  -dissolves  2.7  milliequivalents  at 
156°. 

1  1.  H2O  dissolves  0.7  milliequivalents  at 
218° 

(Melcher,  J.  Am.  Chem.  Soc.  1910,  32.  63.) 

See  also  under  gypsum,  p.  953. 

Maximum  solubility  is  at  37.5°.  (Cameron, 
J.  ohys.  Chem.  1901,  5.  572.) 

Sp.  gr.  of  sat.  CaSO4+Aq  at  15°  =  1.0022. 
(Stolba,  J.  pr.  97.  503.) 

Sp.  gr.  of  sat.  CaSO4+Aq.  at  31°  =  1.0031. 

1  pt.  CaSO4  is  sol.  in  218  pts.  H20  contain- 
ing C02.  (Beyer,  Arch.  Pharm.  (2)  150.  193.) 

SI.  sol.  in  cold  HCl+Aq;  completely  sol.  in 
boiling  dil.  HC1  or  HNO3+Aq.  (Rose,  Pogg. 
95.  108.) 

Solubility  of  CaSO4  in  HCl+Aq. 


100  ccm. 

100  ccm. 

t° 

%  HC1 

dissolve  g. 

t° 

%  HC1 

dissolve  g. 

of  CaS04 

of  CaSO4 

25 

0.77 

0.6405 

25 

6.12 

1.6539 

25 

1.56 

0.8821 

101 

0.77 

1  .  1209 

25 

3.06 

1.2639 

102 

3.06 

3.1780 

25 

4.70 

1  .  5342 

103 

6.12 

4.6902 

(Lunge,  J.  Hoc.  Chem.  Ind.  4.  31.) 
Solubility  in  HNO3+Aq  at  25°. 


g.  HNOs 
par  100  cc. 

g.  CaSO4  per 
100  cc.  solution 

g.  HN03 
per  100  cc. 

g.  CaSO4  per 
100  cc.  solution 

0 

0.208 

6 

1.48 

1 

0.56 

8 

1.70 

2 

0.82 

10 

1.84 

3 

1.02 

12 

1.98 

4 

1.20 

(Banthisch,  J.  pr.  1884,  29.  52.) 

For  s6lubility  in  H2SO4  see  CaH2(SO4)2. 

Solubility  in  H3PO4+Aq  at  25°. 


G.  P2O5  per  1. 

G.  CaSO4  per  1. 

Sp.  gr.  25°/25° 

0.0 

2.126 

5.0 

3.138 

L002 

10.5 

3.734 

1.007 

21.4 

4.456 

1.016 

46.3 

5.760 

1.035 

105.3 

7.318 

1.075 

145.1 

7.920 

1.106 

204.9 

8.383 

1.145 

312.0 

7.965 

1.221 

395.7 

6.848 

1.230 

494.6 

5.573 

1.344 

(Taber,  J.  phys.  Chem.  1906,  10.  628.) 
Solubility  in  formic  acid  at  25°. 
100  cc.  of  solution  of  acid  containing  4% 


SULPHATE,  CALCIUM 


947 


CaCl2+Aq. 

Solubility  of  CaSO4  in  CaCl2+Aq  at  t 


100  ccm. 

100  ccm. 

t° 

% 

CaCl2 

dissolve 
g.  of 

t 

% 

CaCh 

dissolve 
g.  of 

CaSO4 

CaS04 

23 

3.54 

0.1225 

25 

16.91 

0.0702 

24 

6.94 

0.0963 

101.0 

3.54 

0.1370 

25 

10.36 

0.0886 

102.5 

10.36 

0.1426 

25 

15.90 

0.0734 

103.5 

16.91 

0.1301 

dissolve  0.24  g.  CaSO4.     (Banthisch,  J.  pr. 
1884,  29.  52.) 

Solubility  of  CaSO4  in  chloracetic  acid 
at  25°.  100  cc.  of  solution  of  acid  containing 
4%  dissolve  0.22  g.  CaSO4;  10%,  0.25  g. 
(Banthisch,  J.  pr.  1.884,  29.  52.) 

Solubility  in  H2O  is  increased  by  presence 
of  NH4C1  (Vogel,  J:  pr.  1.  196),  ammonium 
succinate  (Wittstein,  Repert.  57.  18), 
(NH4)2S04,  (NH4)2B407  (Popp,  A.  Suppl. 
8.  11);  also  KNO3  (Vogel,  Jun.),  Na2SO4 
(Henry,  J.  Pharm.  12.  31),  NaCl  (Tromms- 
dorf,  N.  J.  Pharm.  18, 1.  234.) 

Decomp.  by  alkali  carbonates  +Aq.  (See 
Storer's  Diet.) 

1  g.  CaSO4  is  sol.  in  162  ccm.  sat.  KCl+Aq 
at  8°;  in  147  ccm.  sat.  NaCl+Aq  at  8.5°;  in 
93  ccm.  sat.  NH4Cl+Aq  at  12.5°;  in  94  ccm. 
sat.  KNO3+Aq;  in  92  ccm.  sat.  NaNO3+Aq; 
in  320  ccm.  sat.  NH4NO3+Aq;  in  54  ccm. 
2/9  sat.  NH4NO3+Aq;  in  about  2000  ccm. 
sat.  K2SO4+Aq.  (Droeze.) 

More  sol.  in  Fe2Clc,  Cr2Cl6,  CuCl2,  ZnCl2-. 
Aq  than  in  H2O,  but  not  more  sol.  in  CaCl2  + 
Aq.    (Gladstone.) 

NH4Cl+Aq. 

1  g.  CaSO4  is  sol.  in  92  ccm.  sat.  NH4C1+ 
Aq  at  13.5°;  in  94  ccm.  l/2  sat.  NH4Cl+Aq  at 
13.5-15.5°;  in  200  ccm.  Vs  sat.  NH4Cl+Aq  at 
13.5°;  in  183  ccm.  Vs  sat.  NH4Cl+Aq  at  100°. 
(Fassbender,  B.  9.  1360.) 

Solubility    of    CaS04    in    25%    NH4Cl+Aq.         Solubility  of  CaSO4  in  CaCl2+Aq  at  t°. 


(Lunge,  I.  c.) 


Solubility  of  CaSO4  in  H2O  containing  various 
amts.  of  CaCl2  at  20°.  100  pts.  H2O  con- 
taining pts.  CaCl2  dissolve  pts.  CaSO4.' 


Pts.  CaCl2 

Pts.  CaS04 

Pts.  CaCh 

Pts.  CaSO4 

0.00 
11.50 
14.39 

0.225 
0.078 
0.063 

19.80 
51.00 
67.05 

0.041 
0.000 
0.000 

(Tilden  and  Shenstone.) 


t° 

%  CaSO4 

t° 

%  CaSO4 

8 
9 
25 
39 

1.030 
1.023 
1.096 
1.126 

60 
80 
120 

1.333 
1.026 
1.000 

(Tilden    and    Shenstone,    Roy.    Soc.    Proc. 
38.  335.) 

t° 

Oa6l2 

% 

CaS04 

t° 

% 

CaCh 

°7 
CaS°O4 

15 
21 

39 

72 

15.00 
14.70 
15.00 
14.90 

0.063 
0.068 
0.091 
0.100 

94 
138 
170 
195 

15.16 
14.70 
14.82 
14.70 

0.110 
0.071 
0.031 
0.022 

Solubility  in  NH4Cl+Aq  increases  with  per- 
centage of  NH4C1,  but  if  solution  contains 
more  than  60  g.  NH4C1  per  1.  more  CaO  dis- 
solves than  SO3.  With  333  g.  NH4C1  per 


L,  the  solution  contains  4.9  g.  SO3  and  4.4  g. 
CaO,  while  the  SO3  content  requires  only 
3.4  g.  CaO.    (Ditte,  C.  R.  1898,  126.  694.) 

Solubility  of  CaSO4  in  NH4Cl+Aq  at  25°. 

Grams  NH4C1  per  liter 

Grams  CaSCh  per  liter 

10.8 
24.4 
46.7 
94.5 
149.7 
198.6 
210.0 
275.0 
325.0 
375.3  (saturated) 

3.90 
5.38 
7.07 
8.80 
10.30 
10.85 
10.88 
10.60 
9.40 
7.38 

(Cameron  and  Brown,  J.  phys.  Chem. 
9.  211.) 

1905, 

(Tilden  and  Shenstone,  I.  c.) 


Solubility  in  CaCl2+Aq  at  25°. 


g.  per  1.  of  solution 

g.  per  1.  of  solution 

CaCb 

CaSO4 

CaCl2 

CaSO4 

0.00 

2.06 

51.53 

1.02 

7.49 

1.24 

97.02 

0.84 

11.96 

1.18 

192.71 

0.47 

25.77 

1.10 

280.30 

0.20 

32.05 

1.08 

367.85 

0.03 

(Cameron  and  Seidell,  J.  phys.  Ch.  1901,  5. 
643.) 


1000  pts.  of  1%  CaCl2+Aq.  dissolve 
1.1414  pts.  CaSO4;  40%  CaCl2,  0.2130  pts. 
CaSO4.  (Orloff,  Chem.  Soc.  1903,  84,  (2) 
211.) 


948 


SULPHATE,  CALCIUM 


Solubility  in  CaO2H2+Aq  at  25°. 

Solubility    of    CaSO4    in    NH4NO3+Aq    at 
25°. 

G.  CaS04l 
perl. 

G.  CaO 
perl. 

Solid  phase 

G.  NH4NOs  per  1. 

G.  CaSO4  per  1. 

0.0 

1.166 

Ca(OH)2 

10 

3.18 

0.391 

1.141 

a 

25 

3.93 

0.666 

1.150 

u 

55 

5.80 

0.955 

1.215 

(I 

100 

7.65 

1.214 

1.242 

(I 

150 

8.88 

1.588 

1.222 

Ca(OH)2  and  CaSO4,  2H2O 

200 

9.85 

1.634 

0.939 

CaSO4,  2H2O 

300 

10.80 

1.722 

0.611 

it 

400 

11.40 

1.853 

0.349 

a 

550 

12.02 

1.918 

0.176 

u 

750 

12.20 

2.030 

0.062 

u 

1000 

11.81 

2.126 

0.0 

(t 

1200 

11.10 

1400 

10  02 

(Cameron  and  Bell,  J.  Am.  Chem.  Soc.  1906, 

OQ     1OO1    A 

-L^wVJ 

saturated 

J-W  .  \J£ 

7.55 

MgCl2+Aq. 

Sol.  in  324  pts.  MgCl2+Aq  (34.1%  MgCl2) 
at  19°.  (Karsten.) 

1  g.  CaSO4  is  sol.  in  146  ccm.  1/9  sat.  MgCl2 
+Aq  at  13.5°.  (Fassbender.) 

1  1.  VQ  sat.  MgCl2+Aq  dissolves  6.83  g. 
CaSO4+2H2O  at  13.5°.  (Droeze.) 


Solubility  of  CaSO4  in  MgCl2+Aq. 


t° 

%  MgCU 

%  CaSO4 

9 
39 

80 

19.7 
11.1 
9.99 

0.765 
2.744 
1.038 

(Tilden  and  Shenstone,  I.  c.) 


Solubility  in  MgCl2+Aq  at  26C 


g.  per  1.  of  solution 

g.  per 

.  of  solution 

MgCh 

CaSO* 

H2O 

MgClj 

CaSO4 

H2O 

0.0 

8.50 
19.18 
46.64 

2.08 
4.26 
5.69 
7.59 

997.9 
996.5 
994.5 
989.1 

121.38 
206.98 
337.0 
441.0 

8.62 

6.57 

2.77 
1.39 

972.2 
949.9 
908.7 
878.6 

(Cameron  and  Seidell,  J.  phys.  Ch.  1901, 
6.  645.) 


1 1.  sat.  MgCl2+Aq  at  25°  containing  476.5 
g.  MgCl2  dissolves  1 .09  g.  CaSO4.  (Cameron 
and  Brown,  J.  phys.  Ch.  1905,  9.  214.) 

NH4NO3+Aq. 

1  g.  CaSO4  is  sol.  in  320  ccm.  sat.  NH4NO3 
+Aq  at  8-9°;  in  54  ccm.  2/9  sat.  NH4NO3  + 
Aq  at  13.5°;  in  103  ccm.  2/27  sat.  NH4NO3+Aq 
at  13.5°.  (Fassbender.) 


(Cameron  and  Brown,  J.  phys.  Chem.  1905, 
9.  213.) 

Ca(N03)2+Aq. 

Solubility    of    CaSO4    in    Ca(NO3)2+Aq    at 
25°. 


Weight  of  1000  cc. 
of  solution 

G. 

Ca(NOs)2per  1. 

G. 

CaSCh  per  1. 

998.1 

0 

2.084 

1013.8 

25 

1.238 

1031.7 

50 

1.196 

1067.3 

100 

1.134 

1136.9  ' 

200 

0.929 

1203.5 

300 

0.759 

1265.6 

400 

0.569 

1328.1 

500 

0.403 

1352.0 

544 

0.346 

(Seidell  and  Smith,  J.  phys.  Chem.  1904,  8. 

498.) 

Mg(N08)2+Aq. 

Solubility   of   CaSO4   in    Mg(NO3)2+Aq    at 
25°. 


Weight  of  1000  cc. 
of  solution  grams 

G.  Mg(NOs)2 
perl. 

G.  CaSO4 
per  1. 

998.1 

0 

2.084 

1020.5 

25 

5.772 

1039.8 

50 

7.884 

1078.6 

100 

9.920 

1149.8 

200 

13.340 

1219.0 

300 

14.000 

1282.1 

400 

14.683 

1355.3 

514 

15.040 

(Seidell  and  Smith,  J.  phys.  Chem.  1904,  8 
497.) 

1  1.  sat.  Mg(NO3)2+Aq  at  25°  containing 
615.1  g.  Mg(NO3)2  dissolves  15.26  g.  CaS04 
(Cameron  and  Brown,  J.  phys.  Ch.  1905,  9 
214.) 


SULPHATE,  CALCIUM 


949 


KNO3+Aq. 

1  g.  CaSO4  is  sol.  in  94  com.  sat.  KNO3+ 
Aq  at  13.5°;  in  82  com.  sat.  KNO3+Aq  at 
15.5°;  in  68  ccm.  nearly  sat.  KNO3+Aq  at 
20°.  (Fassbender.) 

Solubility  in  KNO3+Aq  at  25°. 


KCl+Aq. 

1  g.  CaSO4  is  sol.  in  162  ccm.  sat.  KCl+Aq 
at  8°;  in  295  ccm.  l/b  sat.  KCl+Aq  at  9°. 


Solubility  in  KCl+Aq  at  21' 


Wt.  of  1000  ccm. 

G.  KNO3 

G.  CaSO4 

g-  per  1. 

g.  per  1. 

per  1. 

per  1 

per*! 

KTM 

QQO      1 

On 

2OR1 

1008.1 

12.5 

3.284 

0 

2.05 

60 

6.6 

1015.4 

25.0 

4.080 

10 

3.6 

80 

7.2 

1032.1 

50.0 

5.255 

20 

4.5 

100 

,7.5 

1052.5 

100.0 

6.855 

40 

5.8 

125 

Double  Salt 

10.Q9    A. 

1  CA     0 

7   QH7 

1122  A 

2ao.o 

8.688 

(Ditte,  A.  ch.  1898,  (7)  14.  294. 

1153.9 

260.0 

(   6.278 

a     12.112 

a  Probably  due  to  formation  of  double  salt 

Solubility  in  KI+Aq  at  21°. 

of      calcium      and      potassium      sulphates. 

CaK2(S04)2+H20. 

G.  KI 

per  1. 

G.  CaSO4 
perl. 

G.  KI 

perl. 

G.  CaSO4  per  1. 

(Seidell  and  Smith,  J.  phys.  Chem.  1908.  8. 

496.) 

0 

2.05 

100 

5.1 

NaN03+Aq. 
1  g.  CaSO4  is  sol.  in  92  ccm.  sat.  NaNO3  + 
Aq  at  8.5°;  in  318  ccm.  Vs  sat.  NaNO3+ 
Aq  at  13.5°.     (Fassbender.) 
100  ccm.  sat.  NaNO3+Aq  dissolve  1.086  g. 

10 
20 
40 
60 

80 

2.8 
3.2 
3.9 
4.5 

4.85 

125 
150 

200 
250 
300 

5.45 
5.8 
5.95 
6.00 
Double  salt. 

CaSO4+2H2O;  100  ccm.   Vs  sat.  NaNO3+ 
Aq  dissolve  0.314  g.  CaSO4+2H2O.    (Droeze, 

(Ditte,  I.  c.) 

B.  10.  338.) 

Solubility  in  NaNO3+Aq  at  25°. 


Wt.  of  1000  ccm. 
of  solution  grams 

G.  NaN03 
per  I. 

G.  CaS04 
per  1. 

998.1 

0 

2.084 

1016.3 

25 

4.252 

1034.0 

50 

5.500 

1058.4 

100 

7.100 

1133.6 

200 

8.790 

1191.6 

300 

9.282 

1363.9 

600 

7.886 

1390.4 

655 

7.238 

(Seidell  and  Smith,  J.  phys.  Chem.  1904,  8. 
495.) 

1  1.  sat.  NaNO3+Aq  at  25°,  containing 
[|  668.4  g.  NaNO3,  dissolves  5.52  g.  CaSO4. 
|  (Cameron  and  Brown,  J.  phys.  Ch.  1905,  9. 


NaCl+Aq. 

Sol.  in  122  pts.  sat.  NaCl+Aq.     (Anthon.) 

Insol.  in  sat.  NaCl+Aq,  but  more  sol.  in 
dil.  NaCl+Aq  than  in  H2O.  Maximum 
solubility  in  NaCl+Aq  is  when  the  sp.  gr.  is 
1.033. 

1  g.  CaSO4  is  sol.  in  147  ccm.  of  sat.  XaCl  + 
Aq  at  8.5°;  in  150  ccm.  of  sat.  NaCl+Aq  at 
13.5°;  in  149  ccm.  of  Vs  sat.  NaCl+Aq  at 
13.5°;  in  244  ccm.  of  ]/5  sat.  NaCl+Aq  at 
13.5°.  (Fassbender.) 

100  ccm.  sat.  NaCl+Aq  dissolve  0.6785  g. 
CaSO4+2H2O  at  8.5°;  0.6665  g.  CaSO4  + 
2H2O  at  13.5°.  100  ccm.  Vs  sat.  NaCl+Aq 
dissolve  0.671  g.  CaSO4+2H2O  at  13.5°; 
sat.  NaCl+Aq  dissolve  0.4085  g.  CaSO4  + 
2H2O  at  13.5°.  (Droeze.) 


214.) 
Solubility  in  KBr+Aq  at  21°. 

Solubility  of  CaSO4  in  NaCl+Aq  at  t°. 

G.  KBr 
per  1. 

G.  CaS04 
perl. 

G.  KBr 
perl. 

G.  CaSO4perl. 

t° 

Nabl 

CaS°04 

t° 

% 

NaCl 

% 

CaSCh 

0 

10 
20 
40 
60 

80 

2.05 

3.1 
3.6 
4.5 
5.2 
5.9 

100 
125 

150 
200 
250 

6.3 
6.7 
7.0 
7.3 
Double  salt. 

20 
44 
67 
85 
101 

19.90 
19.93 
19.95 
19.90 
20.08 

0.823 
0.830 
0.832 
0.823 
0.682 

130 
165 
169 
•179 
225 

19.92 
20.04 
20.05 
20.10 
21.00 

0.392 
0.250 
0.244 
0.229 
0.178 

(Tilden    and    Shenstone,    Roy.    Soc.    Proc. 
38.  331.) 

(Ditte,  A.  ch.  1898,  (7)  14.  294.) 

950 


SULPHATE,  CALCIUM 


Solubility  of  CaSO4  in  NaCl+Aq  at  t°. 


100  ccm. 

100  ccm. 

t 

l&l 

dissolve 
g.  of 

t° 

A 

dissolve 
g.of 

CaSO4 

CaSO4 

21.5 

3.53 

0.5115 

17.5 

17.46 

0.7369 

19.5 

7.35 

0.6429 

101.0 

3.53 

0  .  4891 

21 

11.12 

0.7215 

102.5 

14.18 

0.6248 

18 

14.18 

0.7340 

103 

17.46 

0.6299 

(Lunge,  J.  Soc.  Chem.  Ind.  4.  31.) 

100  pts.  H2O  containing  pts.  NaCl  dissolve 
pts.  CaSO4  at  20°. 


Pts. 

Pts. 

Pts. 

Pts. 

Pts. 

Pts. 

NaCl 

CaSO4 

NaCl 

CaSO4 

NaCl 

CaS04 

0.00 

0.225 

5.05 

6.34 

24.40 

0.820 

0.52 

0.301 

10.00 

7.38 

35.10 

0.734 

2.03 

0.441 

20.00 

0.823 

35.86 

0.709 

5.02 

6.15 

(Tllden  and  Shenstone.) 


Solubility  in  NaCl+Aq  at  26°. 


g.  per  1. 


NaCl      CaS04 


0.00 
9.11 

143.99 
148.34 


2.12 
6.66 
7.18 
7.16 


wt.  of 

1  cc. 

solution 


0.9998 
1.0644 
1.0981 
1.012 


g.  per  1. 


NaCl       CaS04 


176.50 
228.76 
264.17 
320.49 


7.12 
6.79 
6.50 
5.72 


wt.  of 

1  cc. 

solution 


1.1196 
1 . 1488 
1 . 1707 
1.2034 


(Cameron,  J.  phys.  Ch.  1901,  6.  556.) 
Solubility  in  NaCl+Aq  at  15°. 


G.  CaSCh  per  1. 


2.3 
2.5 
3.1 
3.7 

4.8 
5.6 
7.4 


G.  NaCl  per  1. 


0.6 

1.1 

5.1 

10.6 

31.1 

51.4 

139.9 


Solubility  in  NaCl+Aq. 


30° 

52° 

70° 

82° 

d 

I-: 
O 

E 

sL 

£ 

iL 

5^ 

§L 

d  a 

d 

da 

d 

d  a 

d 

0.5 

2.5 

0.5 

2.3 

0.5 

2.2 

0.0 

2.07 

10.3 

3.6 

1.1 

2.4 

10.0 

3.4 

1.0 

2.18 

30.3 

5.0 

5.0 

2.9 

29.6 

4.9 

5.0 

2.65 

47.3 

6.1 

10.1 

3.5 

48.8 

5.8 

10.1 

3.30 

73.4 

6.9 

29.6 

5.0 

132.7 

7.4 

29.5 

4.68 

126.9 

7.3 

48.3 

5.8 

195.0 

7.6 

48.8 

5.54 

192.4 

7.7 

75.7 

6.6 

74.9 

6.23 

131.6 

7.1 

128.7 

7.00 

195.9 

7.4 

195.1 

7.15 

(Cameron,  J.  phys.  Ch.  1901,  6.  562.) 

1  1.  sat.  NaCl+Aq  at  25°  containing  318.3 
g.  NaCl  dissolves  5.52  g.  CaSO4.  (Cameron 
and  Brown,  J.  phys.  Ch.  1905,  9.  214.) 


Solubility  in  NaCl+Aq. 


G.  NaCl  per  1. 

of  NaCl+Aq 

G.  anhydrous  CaSO4  dissolved 
per  litre 

at  14° 

at  20° 

0.0 

1.70 

2.10 

2.925 

2.32 

2.70 

5.850 

2.79 

3.15 

11.70 

3.41 

3.75 

14.62 

3.68 

4.00 

29.25 

4.40 

4.70 

58.50 

5.72 

6.00 

87.75 

6.58 

6.85 

102.3 

6.90 

7.15 

117.0 

7.10 

7.30 

131.6 

7.20 

7.30 

146.2 

7.10 

7.13 

160.8 

7.00 

7.05 

175.6 

6.80 

6.80 

204.7 

6.30 

6.30 

234.0 

5.90 

5.90 

263.2 

5.50 

5.52 

292.6 

5.30 

5.30 

(Cameron,  J.  phys.  Ch.   1901,  6.  559.) 
Solubility  in  NaCl+Aq  at  26°. 


(d'Anselme,  Bull.  Soc.  1903,  (3)  29.  373.) 
Solubility  in  NaCl+Aq. 


NaCl  in  100  g.  H2O 


0.0000 

9.4307 
15.2056 
15.6859 
18.8570 
25.0478 
29.3509 
36.5343 


CaSCh  in  100  g.  H2O 


G.  NaCl  in 
100  cc.  solution 


0.2126 
0.6886 
0.7581 
0.7575 
0.7605 
0.7439 
0.7219 
0.6515 


0.00 

2.44g. 

4.77g. 

9.50g. 
14.22g. 
23.15g. 
31.30g. 


G.  CaSO4+2H20 


0.200g. 

0.635g. 
0.826g. 
1.056  g. 
1.193g. 
1.275g. 
1.583g. 


(Cameron,  J.  phys.  Ch.  1901,  5.  564.) 


(Cloez,  Bull.  Soc.  1903,  (3)  29.  167.) 


SULPHATE,  CALCIUM 


951 


Solubility  in  NaCl+Aq  at  t°. 
When  a  sat.  solution  of  NaCl  is  shaken 
with  a  mixture  of  solid  NaCl  and  CaSO4+ 
2H2O,  the  calcium  sulphate  dissolved,  cal- 
culated from  the  amount  of  CaO  in  solution,  is 
always  greater  than  that  calculated  from  the 
sulphuric  acid  in  solution.  Similar  results  are 
obtained  when  solid  calcium  sulphate  alone  is 
shaken  with  a  sat.  solution  of  NaCl. 


0 
10 
25 
40 
50 
60 
62. 
65 
71 
75 
85 


In  100  g.  of  the  solution 


01 


15.253 
15.920 
15.967 
16.123 
16.270 
16.324 
16.361 
16.459 
16.486 
16.524 
16.670 
17.128 


CaSO4  calc. 
from  CaO 


0.4464 
0.4477 
0.4609 
0.4938 
0.5093 
0.5305 

0^5435 
0.5578 
0.5603 
0.5399 
0.4086 


CaSO4  calc. 
from  SOi 


0.4334 
0.4426 
0.4542 
0.4730 
0.4832 
0.5047 
0.5091 
0.3749 
0.3631 
0.3587 
0.3519 
0.3414 


(Arth,  Bull'.  Soc.  1906,  (3)  35.  780.) 

Within  a  temp,  range  from  25°-80°  CaSO4 
CaSO4  forms  no  double  salt  in  solutions  oJ 
NaCl.  At  any  concentration  with  respect  to 
the  latter  maximum  solubility  occurs  with  155 
g.  NaCl  per  1.  and  amounts  to  7.3  g.  CaSO4  at 
80°.  (Cameron,  J.  phys.  Chem.  1907,  11. 
496.) 

See  also  under  Gypsum,  p.  653. 

Solubility  of  CaSO4  in  NaCl+Aq  in  contact 
with  solid  Ca(HCO3)2. 


G.  CaSO4 
perl. 


1.9298 
2.7200 
3.4460 
5.1560 
6.4240 
5.2720 
4.7860 
4.4620 


G.  Ca(HCOs)» 
per  1. 


0.0603 
0.0724 
0.0885 
0.1006 
0.0603 
0.0563 
0.0482 
0.0402 


G.  NaCl 

perl. 


0.000 

3.628 

11.490 

39.620 

79.520 

121.900 

193.800 

267.600 


(Cameron  and  Seidell,  J.  phys.  Chem.  1901, 
6.  653.) 


(NH4)2S04+Aq. 

Sol.  in  287  pts.  (NH4)2SO4+Aq  (1:4). 
(Fresenius,  Z.  anal.  30.  593.) 

1  g.  CaSO4  is  sol.  in  327  ccm.  (NH4)2SO4 
+Aq  at  9°;  in  369  ccm.  l/7  sat.  (NH4)2SO4+ 
Aq  at  13.5°.  (Fassbender.) 

Solubility  in  sat.  (NH4)2SO4,  or  Na2SO4  is 
the  same  as  in  H2O.  (Droeze,  B.  10.  330.) 


Solubility  in  (NH4)2SO4+Aq  at  25°. 


g.  per  1.  solution 


0.00 

0.129 

0.258 

0.821 

1.643 

3.287 


0.208 
0.204 
0.199 
0.181 
0.166 
0.154 


wt.  of 
100  cc. 
solution 


99.91 
99.91 
99.92 
99.95 
99.99 
100.10 


6.575 
13.15 
26.30 
84.9 

169.8 

339.6 


0.144 
0.146 
0.162 
0.233 
0.333 
0.450 


wt.  of 
100  cc. 
solution 


100.36 
100.82 
101.76 
105.34 
110.32 
119.15 


(Sullivan,  J.  Am.  Chem.  Soc.  1905,  27.  529.) 
Solubility  in  (NH4)2SO4+Aq  at  50°. 


Sp.  gr. 

(NHf)2S04 
perl. 

Cal'cu 

perl. 

Solid  phase 

0 

2.168 

1.0026 

15.65 

1.609 

1.0113 

30.67 

1.750 

1.0440 

91.6 

2.542 

1.0819 

160.4 

3.402 

.1108 

221.6 

4.068 

CaS04+2H20 

.1385 

280.6 

4.690 

.1653 

340.6 

5.084 

.1972 

415.6 

5.336 

.1964 

416.5 

5.354 

.2043 

.2187 

428.4 
479.4 

4.632 
3.524 

CaSO4,  (NH4)2SO4-t- 

.2437 

530.8 

2.152 

2H2O 

.2480 

558.0 

1.986 

.2502 

564.7 

1.98 

1.2508 

566.0 

1.08 

(NH4)2SO4 

1.2510 

566.7 

0 

(Bell  and  Taber,  J.  phys.  Chem.  1906,  10. 
120.) 

Solubility  of  CaSO4  in  (NH4)2S04+Aq  at  t°. 

Excess  of  (NH4)2S04  Excess  of  CaSO4 


6 
40.5 

58 

78 

100 


0.1529 
0.1569 
0.1662 
0.1968 
0.2546 


*3 

55 


41.82 
44.55 
46.07 
47.51 
49.45 


3 
31 
60 
75 

80 

84 

100 


0.3782 
0.4070 
0.5083 
0.5898 
0.6108 
0.5725 
0.4895 


36.62 
35.50 
34.97 
34.86 
34.88 
32.40 
25.97 


(Barre,  C.  R.  1909,  148.  1605.) 

The  solubility  of  CaSO4  in  H2O  is  consider- 
ably increased  by  the  presence  of  (NH4)2SO4 


952 


SULPHATE,  CALCIUM 


but  decreased  by  the  presence  of  K2S04. 
(Barre,  C.  R.  1909,  148.  1606.) 

CuSO4+Aq. 
Solubility  in  CuSO4+Aq  at  25°. 

Solubility  in  K2SO4+Aq  at  25°. 

g.  per  1. 

wt.  of  1  cc.  of 
solution 

K2S04 

CaSO 

4 

0.0 
4.88    • 
5.09 
9.85 
19.57 
28.35 
30.66 
32.47* 

2.08 
1.60 
1.56 
1.45 
1.49 
1.55 
1.57 
1.58 

0 
1 
1 
1 
0 
1 
1 

.9981 
.0036 
.0038 
.0075 
.151 
.0229 
.0236 

Sp.  gr.  of  the 
solution  25°/25° 

g.  CuSp4 
per  1. 

g.  CaSO4 
perl. 

.002 
.005 
.007 
.009 
.016 
.021 
.030 
.041 
.051 
.061 
.098 
.146 
.192 
.218 

1.144 
3.564 
6.048 
7.279 
14.814 
19.729 
29.543 
39.407 
49.382 
58.880 
97.950 
146.725 
196.021 
224.916 

2.068 
1.986 
1.944 
1.858 
1.760 
1.736 
1.688 
1.718 
1.744 
1.782 
1.931 
2.048 
2.076 
2.088 

*Solid  phase  syngenite. 
(Cameron  and  Breazeale,  J.phys.  Ch.  1904,  8. 
335.) 

Solubility  in  K2SO4+Aq.  at  25°. 
In  1000  g.  of  the  solution 
mole  K2SO4            mole  CaSO4 
3.223                       0.223 
(D'Ans,  Z.  anorg.  1909,  62.  151.) 

Solubility  of  CaSO4  in  K2SO4+Aq  at  t°. 

Excess  of  K2SO4 

Excess  of  CaSO4 

(Bell  and  Taber,  J.  phys,  Ch.  1907,  11.  637.) 

MgS04+Aq. 
Insol.  in  sat.  MgSO4+Aq. 
1  g.  CaSO4  is  sol.  in  1162  ccm.   Vio  sat. 
MgSO4+Aq  at   13.5°.      (Fassbender,   B.   9. 
1360.) 
^  Sol.  in  635  pts.  sat.  MgSO4+Aq  at  19°. 
(Karsten.) 
Absolutely  insol.  in  sat.  MgSO4+Aq,  and 

t° 

4 

^3 
M 

4 

£§GC 

M 

0* 
18 
51 
80 
99 

0.1296 
0.1531 
0.1754 
0.1922 
0.1980 

2.00 
2.79 
4.21 
5.00 
5.39 

0.0229 
0.0271 
0.0300 
0.0349 
0.0371 

6.99 
9.81 
14.18 
17.55 
19.70 

of  MgSO4.    (Droeze,  B.  10.  340.) 

1  1.  Vio  sat.  MgSO4+Aq  dissolves  0.86  g. 
CaSO4+2H2O.    (Droeze.) 


Solubility  in  MgSO4+Aq  at  25°. 


g.  per  1. 

Sp.  gr. 

at 
25°/25° 

g.  per  I. 

Sp.  gr. 
at 
25°/25° 

MgSO4 

CaSO4 

MgSO4 

CaS04 

0.0 

2.046 

1.0032 

149.67 

1.597 

1.1377 

3.20 

1.620 

1.0055 

165.7 

1.549 

1.1479 

6.39 

1.507 

1.0090 

171.2 

1.474 

1.1537 

10.64 

1.471 

1.0118 

198.8 

1.422 

1.1813 

21.36 

1.478 

1.0226 

232.1 

1.254 

1.2095 

42.68 

1.558 

1.0419 

265.6 

1.070 

1.2382 

64.14 

1.608 

1.0626 

298.0 

1.860 

1.2624 

85.67 

1.617 

1.0833 

330.6 

0.647 

1.2877 

128.28 

1.627 

1.1190 

355.0 

0.501 

1.3023 

(Barre,  C.  R.  1909,  148.  1606.) 

Ag2S04+Aq. 

1  1.  of  the  solution  contains  2.31  g.  CaSO4 
+7.23  g.  Ag2SO4  =  9.54  g.  mixed  salts  at  17°. 
Sp.  gr.  =  1.0083. 

1 1.  of  the  solution  contains  2.61  g.  CaSO4-f- 
8.11  g.  Ag2SO4  =  10.72  g.  mixed  salts  at  25°. 
Sp.  gr.  =  1.010.  (Euler,  Z.  phys.  Ch.  1904, 
49.  313.) 

Na2S04+Aq. 

1  g.  CaSO 4  is  sol.  in  398  ccm.  sat.  Na2SO4  + 
Aq  at  10.5°. 

Solubility  of  CaSO4  in  Na2SO4+Aq  at  22° 


(Cameron  and  Bell,  J.  phys.  Ch.  1906,  10. 
210.) 


G.  CaSC>4  per  1. 

G.  Na2S04  per  1. 

2.084 

0.000 

1.583 

2.771 

1.433 

13.820 

1.408 

16.360 

1.569 

39.310 

1.841 

77.320 

2.185 

133.00 

2.414 

193.800 

*2.578 

*222.580 

*Both  (JaSO4  and  Na2iSO4  as  solid  phases  in 
contact  with  the  solution. 
(Cameron  and  Seidell,  J.  phys.  Chem.  1901,  5. 
650.) 


SULPHATE,  CALCIUM 


953 


Solubility  in  Na2SO4+Aq  at  25°. 

Solubility    in     N/200    KHC2H4O6+Aq+ 

o  /o  tartanc  acid  —  U.Jooo  g.  Ua&u4  per  1UU 

wt.  of  1000  ccm. 
of  solution  grams 

g.  Na2SO4  per  1. 

* 

g.  CaSO4  per  1. 

g.  solution. 
Solubility     in      10%      alcoholic      N/400 

1001.26 
1007  59 

2.390 
9  535 

1.650 
1  457 

KHC2H4O6+5%    tartaric     acid  =  0.1086     g. 
CaSO4  in  100  g.  solution.    (Magnanini.) 

1011.45 
1020.46 

14.132 
24.369 

1.388 
1.471 

Insol.  in  methyl  acetate.     (Naumann,  B. 
1909,  42.  3790);  ethylacetate.    (Naumann,  B. 

1031.48 

36.979 

1.563 

1910,  43.  314.) 

1039.12 
1079.47 

46.150 
94.220 

1.650 
1.980 

Solubility  in  sugar  +Aq  at  t°. 

1096.47 

115.084 

2.096 

G.  CaSO4  dissolved  in  1  1.  sugar  solutions 

1142  66 

146  612 

2  234 

% 

1176.47 

205.105 

2.503 

sugar 

30° 

40° 

50° 

60° 

70° 

80° 

1212.00 

257  .  100 

.650 

o 

• 

2  157 

1  730 

1  730 

1  652 

1  710 

(Cameron    and    Breazeale,    J.    phys.    Chem. 

10 

2.041 

1.730 

1.730 

1.574 

1.574 

1.613 

1904,  8.  340.) 

20 

1.808 

1.652 

1.419 

1.380 

1.419 

1.263 

27 

1.550 

1.438 

1.361 

1.283 

1.283 

0.972 

1   1.   sat.   Na2SO4+Aq  at  25°  containing 
254.09,    Na2SO4    dissolves    2.58    g.  CaSO4.. 
(Cameron  and  Brown.  J.  phys.  Ch.  1905,  9 

214.) 

35 
42 
49 
55 

1.263 
1.030 

1.050 

0^564 

0.486 

1.088 
0.777 
0.739 
0.505 

1.108 
0.816 
0.564 
0.486 

0.914 
0.855 
0.603 
0.369 

0^729 
0.486 
0.330 

and  accelerated  by  cone,  solution  of  sodium, 
potassium,  ammonium  and  magnesium  sul- 
phates. (Rohland,  Z.  Elektrodiem.  1908, 
14.  422.) 

More  than  10  times  as  much  CaSO4  dis- 
solves in  sat.  Na2S2O3  + Aq  as  in  H2O.  (Diehl. 

Insol.  in  alcohol,  of  0.905  sp.  gr.  or  less. 
(Anthon,  J.  pr.  14.  125.) 

Solubility  in  10%  alcohol  =  0.0970  g. 
CaSO4  per  100  g.  solution.  (Magnanini, 
Gazz.  Ch.  it.  1901,  31.  (2)  544.) 

Sol.  in  dil.  alcoholic  solutions  of  NH4NO3, 
KN03,  NaN03,  NH4C1,  KC1,  and  NaCl. 
(Margueritte,  C.  R.  38.  308.) 

Sol.  to  considerable  extent  in  NH4C2H3O2 
+  Aq,  especially  if  freshly  pptd.  More  sol. 
in  NH4C2H3O2+Aq  than  in  NH4Cl+Aq. 
(Weppen,  J.  pr.  11.  182.) 

More  sol.  in  NH4C2H3O2  +  Aq  than  in  other 
NH4  salts.  (Cohn,  J.  pr.  (2)  35.  43.) 

More  sol.  in  NaC2H3O2+Aq  or  KCl+Aq 
than  in  H2O.  (Mulder.) 

Solubility  in  N/200  potassium  hydrogen 
tartrate +Aq  =  0.2323  g.  CaSO4  per  100  g. 
solution.  (Magnanini,  Gazz.  ch.  it.  1901,  31. 
(2)  544.) 

72.61  millimols.  per  1.  of  CaSO4+2H2O  are 
sol.  at  25°  in  ammonium  citrate +Aq  (con- 
centration =  0.5  millimols.  per  1.) 

36.39  millimols  per  1.  of  CaSO4-f2H2O  are 
sol.  at  25°  in  sodium  citrate  -{-Aq.  (Con- 
centration =  0.25  millimols  per  1.  (Rindell, 
Z.  phys.  Ch.  1910,  70.  452.) 

100  pts.  glycerine  dissolve  0.957  pt.  CaSO4 
+2H2O,  and  solubility  increases  with  the 
temp.  (Asselin,  C.  R.  76.  884.) 

100  g.  glycerine  (sp.  gr.  1.256)  dissolve 
5.17  g.  CuSO4  at  15-16°.  (Ossendowski, 
Pharm.  J.  1907.  79.  575.) 

Solubility  in  10%  alcoholic  N/200 
KHC2H4O6+Aq=  0.0866  g.  CaSO4  per  100 
g.  solution. 


(Stolle,  Z.  Ver.   Zuckerind,    1900,   60.   331). 

Min.  Anhydrite. 

+2H2O.    Min.  Gypsum. 

Gypsum.  A  sat.  aq.  solution  of  gypsum 
of  particles  not  less  than  2^  contains  2.085  g. 
CaS04  per  litre  at  25°. 

A  sat.  aq.  solution  of  gypsum  of  particles 
not  smaller  than  0.3/u.  contains  2.476  g.  CaSO4 
per  liter  at  25°.  (/x =0.0001  cm.)  (Hulett 
and  Allen,  Z.  phys.  Ch.  1901,  37.  391  and 
393.) 

Solubility  in  H2O  at  t°. 


t° 

g.  CaSCh  in  100 
ccm.  of  the 
solution 

Density  of  the 
solution  at  t° 

o' 

0.17590 

1.001970 

10 

0.19285 

1.001727 

18 

0.20160 

1.000590 

25 

0.20805 

0.999109 

30 

0.23935 

0.997891 

35 

0.20960 

0.996122 

40 

0.20970 

0.994390 

45 

0.20835 

0.992370 

55 

0.20095 

0.987960 

65.3 

0.19320 

0.982560 

75 

0.18475 

0.977724 

100 

0.16195 

(Hulett  and  Allen,  J.  Am.  Chem.  Soc.  1902, 
24.  674.) 

1  1.  H2O  dissolves  2.13  g.  CaSO4+2H20  at 
25°.  (Euler,  Z.  phys.  Ch.  1904,  49.  314.) 

2023  mg.  are  dissolved  in  1 1.  of  sat.  solution 
at  18°.  (Kohlrausch,  Z.  phys.  Ch.  1908,  64. 
168.) 

1  1.  H2O  dissolves  2.267  g.  CaSO4+2H2O 
at  0°;  2.684  g.  at  35°;  2.662  g.  at  50°;  and 
2.155  g.  at  100°.  (Cavazzi,  C.  C.  1905,  I. 
1693.) 


954 


SULPHATE,  CALCIUM  HYDROGEN 


1  1.  H2O  dissolves  29.5  milliequivalents  at 
18°;  30  at  50°;  23.3  at  100°.  (Melcher,  J 
Am.  Chem.  Soc.  1910,  32.  63.) 

See  also  under  CaSO4. 

Solubility  of  pulverized  gypsum  in  NaCl+Aq 
at  23°. 


Grams  gypsum 

G.  NaCl  per  1. 

G.  CaSO4  per  1. 

2.99 

0.99 

2.37 

3.82 

4.95 

3.02 

4.48 

10.40 

3.54 

6.31 

30.19 

4.97 

7.51 

49.17 

5.94 

8.53 

75.58 

6.74 

9.42 

129.50 

7.50 

9.17 

197.20 

7.25 

8.88 

229.70 

7.03 

7.19 

306.40 

5.68 

6.79 

315.55 

5.37 

(Cameron,  J.  phys.  Chem.  1901,  6.  559.) 
See  also  under  CaSO4. 


Plaster  of  Paris  contains 
according  to  Chatelier  (C.  C.  1889,  1.  203). 


Calcium  hexahydrogen  sulphate,  CaH6(SO4)4. 
Decomp.  by  H2O.     (Schultz,  Pogg.  133. 
137.)  ^ 

Calcium  cupric  potassium  sulphate. 

Ca2K2Cu(SO4)4-f2H2O. 
(D'Ans,  B.  1908,  41.  1778.) 

Calcium  magnesium  potassium  sulphate. 
2CaS04,  MgS04,  K2SO4+2H2O. 

Min.  Polykalite.  Sol.  in  H2O  with  residue 
of  CaSO4. 

4CaSO4,  MgSO4  K2SO4+2H20.  Min. 
Krugite.  Decomp*  by  H2O. 

Calcium  potassium  sulphate,  CaK2(SO4)2+ 
H2O. 

Min.  Syngenite.  Sol.  in  400  pts.  H2O. 
(Zepharovitch.)  Less  sol.  than  K2SO4. 
Decomp.  by  heating  with  separation  of  CaSO4 
Decomp.  by  H2O  until  25  g.  K2SO4  are  dis- 
solved in  a  litre,  after  which  there  is 
composition.  (Ditte,  C.  R.  84.  86.) 

Easily  sol.  in  dil.  acids.    (Phillips.) 


no  de- 


Solubility  of  syngenite,  CaK2(SO4)2+H2O  in 
K2SO4+Aq  at  25°. 


Calcium  hydrogen  sulphate,  CaH2(SO4)2. 
100  pts.  H2SO4  of  1.82  sp.  gr.  dissolve  about 
2  pts.  CaSO4;  100  pts.  fuming  H2SO4  dissolve 
10.17  pts.  CaSO4  (Struve,  Z.  anal.  9.  34);  100 
pts.   H2SO4  dissolve  2.5  pts.   CaSO4    (Lies- 
Bodart   and   Jacquemin,    C.    R.    46.    1206); 
CaSO4  is  precipitated  by  H2O  from  H2SO4 
solution. 
100  pts.   boiling   H2SO4  dissolve    10  pts. 
CaSO4.    (Schultz,  Pogg.  133.  137.) 

Solubility  :  of  CaSO4  in  H2SO4+Aq. 

Wt.  of  1000  ccm. 
of  solution  grams 

g.  K2S04  per  1. 

g.  CaSO4  per  1. 

1013.08 
1015.78 
1020.01 
1024.54 
1036.82 
1058.10 
1085.91 

16.31 
19.87 
25.01 
30.83 
46.99 
75.45 
112.87 

*1.495 

1.529 
1.537 
1.565 
0.810 
0.451 
0.330 

*In    first    four    determinations    syngenite 
completely  decomposed. 
(Cameron    and    Breazeale,    J.    phys.    Chem. 
1904,  8.  339.) 

This  double  salt  is  stable  between  0°  and 
)9°  in  the  presence  of  an  excess  of  either 
CaSO4  or  K2S04.    In  this  temp,  interval  the 
double  sulphate,  2CaSO4,  K2SO4,  3H2O  de- 
scribed by  Ditte  (C.  R.  84.  867)  does  not 
exist.    (Barre,  C.  R.  1909,  148.  1607.) 
Ca2K2(SO4)3+3H2O.      Decomp.    by    cold 
H2O.    (Ditte,  C.  R.  84.  867.) 
5CaS04,    K2SO4+H2O.      Slowly   decomp. 
by  H2O.     (van't  Hoff  and  Geiger,  B.  A.  B. 
1904.  935.) 

Calcium  potassium  zinc  sulphate, 

Ca2K2Zn(SO4)4+2H2O. 
(D'Ans,  B.  1908,  41.  1778.) 

wt.  of  1000 
ccm.  of 
solution  at 
25° 

g.  H2S04 
per  1. 

g.  CaSO4  per  1.  at 

25° 

35° 

43° 

999.1067 
1002.493 
1002.553 
1005.091 
1009.787 
1030.151 
1043.470 
1075.613 

1113^392 
1141.755 
1168.143 

0.00 
0.48 
4.87 
8.11 
16.22 
48.67 
75.00 
97.35 
146.01 
194.70 
243.35 
292.02 

2.126 
2.128 
2.144 
2.203 
2.382 
2.727 
2.841 
2.779 
2.571 
2.313 
1.901 
1.541 

2^209 
2.451 

3^397 

3^606 
3.150 

2.145 
2.236 
2.456 
2.760 
3.116 
3.843 
4.146 

4!i39 
3.551 
2.959 
2.481 

(Cameron   and   Breazeale,    J.    phys.    Chem. 
1903,  7.  574.) 

100  pts.  hot  cone.  H2SO4  dissolve  approx. 
10  pts.  CaSO4.  (Rohland,  Z.  anorg.  1910,  66. 
206.) 

Decomp.  by  H2O. 


Calcium  rubidium  sulphate,  Ca2Rb2(SO4)3. 

(D'Ans,  B.  1907,  40.  4913.) 

+3H2O.    Decomp.  by  H2O.    (Ditte,  C.  R. 
84.  86.) 

CaRb2(SO4)2+H2O.    (D'Ans.) 


SULPHATE,  CEROUS 


955 


Calcium  sodium  sulphate,  CaNa2(SO4)2. 

Min.  Glauberite.  Gradually  sol.  in  H2O, 
but  crystals  of  CaSO4+2H2O  soon  separate 
out.  (Fritzsche.) 

Insol.  in  alcohol,  and  cone.  NaC2H3O2  + 
Aq;  decomp.  by  H2O.  (Folkhard,  C.  N.  43. 
6.' 

CaNa4(SO4)3+2H2O.  Decomp.  by  H2O. 
(Fritzsche.) 

Calcium  titanium  sulphate,  CaS04,  Ti(SO4)2. 
Ppt.;  decomp.  by  H2O  giving  titanic  acid. 
(Weinland,  Z.  anorg.  1907,  54.  254.) 

Calcium  uranium  sulphate. 

Min.  Uranochalcite. 

Min.  Medjidite.  Easily  sol.  in  dil.  HC1-J- 
Aq. 

Cerous  sulphate,  Ce2(SO4)3. 

Anhydrous  cerous  sulphate  is  much  more 
sol.  in  H2O  than  the  hydrated  salt. 

Easily  sol.  in  cold  H^O  if  added  thereto  in 
small  amounts.  If  large  amount  of  Ce2(SO4)3 
is  treated  with  a  little  H2O  it  hardens  with 
evolution  of  heat,  and  becomes  very  difficultly 
soluble.  100  pts.  H2O  dissolve  161  pts. 
Ce2(SO4)3  at  0°  and  17.86  pts.  at  19°. 

Ce2(SO4)3+Aq  sat.  in  cold  deposits 
Ce2(SO4)3  at  75°,  and  only  2.25  pts.  remain  in 
solution  at  100°.  (Jolin,  Bull.  Soc.  (2)  21. 
536.) 

100  pts.  H2O  dissolve  8.31  pts.  Ce2(SO4)3  at 
20°;  8.08  pts.  at  45°;  4.95  pts.  at  60°;  0.504 
pt.  at  100°.  (Biihrig,  J.  pr.  (2)  12.  240.) 

60  pts.  anhydrous  salt  dissolve  quickly  at 
0-3°  in  100  pts.  H2O. 

At  15°  the  solution  solidifies,  and  the  mother 
liquor  contains  only  27.88%  Ce2(SO4)3.  At 
15°  the  maximum  attainable  strength  is 
31.62%  Ce2(SO4)3.  (Brauner,  Chem.  Soc.  53. 
357.) 

100  pts.  H2O  dissolve  10.747  pts.  Ce2(SO4)3 
at  16°;  9.648  pts.  at  19°;  6.949  pts.  at  33°. 

The  solubility  of  Ce2(SO4)3  in  H2O  is  dimin- 
ished by  the  addition  of  (NH4)2SO4,  K2SO4 
or  Na2SO4.  (Barre,  C.  R.  1910,  151.  872.) 

Sp.  gr.  of  Ce2(SO4)3+Aq  was  found  to  be  con- 
stant whether  Ce2(SO4)3  or  Ce2(SO4)3  + 
8H2O  was  used.  The  following  results 
were  obtained  at  15°. 


Pts. 
Ce2(S04)3to 
100  pts.  H2O 

Sp.  gr. 

Pts. 
Ce2(SO4)sto 
100  pts.  H2O 

Sp.  gr. 

3.17 
6.11 
8.35 
9.61 
10.55 
11.66 

.03005 
.05812 
.07910 
.09085 
.09939 
.  10987 

12.66 
14.56 
15.64 
21.19 
31.62 

1.11917 
1  .  13665 
1  .  14623 
1  .  19640 

1.28778 

Per  100  pts.  H2O 

(NH4)2S04 

Ce2(SO4)3 

0.00 

10.747 

3.464 

1.026 

9.323 

0.782 

19.240 

0.748 

29.552 

0.701 

45.616 

0.497 

55.083 

0.194 

63.920 

0.090 

72.838 

0.035 

(Brauner,  Chem.  Soc.  53.  357.) 


4.5  pts.   Ce2(SO4)3   dissolve   in    100   pts. 
H2SO4.     (Wyrouboff,  Bull,  Soc.  (3)  2.  745.)  j 


Solubility  in  (NH4)2SO4+Aq  at  16°. 


(Barre,  A.  ch.  1911,  (8)  24.  252.) 


Solubility  in  Na2SO4+Aq  at  19°-20°. 

Per  100  pts.  H2O 

Na2S04 

Ce2(S04)3 

0.00 

9.64 

0.328 

0.637 

0.684 

0.259 

1.091 

0.0937 

1.392 

0.057 

1.699 

0.0303 

2.640 

0.012 

3.589 

0.0065 

5.660 

0.0046 

7.710 

0.0037 

(Barre,  A.  ch.  1911,  (8)  24.  251.) 


Solubility  in  K2SO4+Aq  at  16°. 


Per  100  pts.  H2O 


K2SO4 

Ce2(SO4)3 

0.00 
0.178 
0.510 
0.726 
1.290 

10.747 
0.956 
0.432 
0.250 
0.0419 

(Barre,  A.  ch.  1911,  (8)  24.  248.) 


+4H2O.    100  g.  H2O  dissolve  at: 
35°    -40°      50°      57° 
8.5     6.04    3.43    2.34  g.  Ce2(SO4)3. 

65°      70°     82°    100.5°  bpt.  of  sat.  solution. 
1.883   1.38   1.01    0.43  g.  Ce2(SO4)3. 

(Koppel,  Z.  anorg.  1904,  41.  399.) 


956 


SULPHATE,  CEROCERIC 


+5H20. 

100  pts.  H2O  dissolve  pts.  Ce2(SO4)3  at  t°. 


t° 

Pts.  Ce2(SO4)3 

100 
80 
60 
50 
40 

0.775 
1.70 
3.45 
5.56 

8.20 

(Muthmann  and  Rolig,  Z.  anorg.  1898,  16. 
456.) 

100  g.  H2O  dissolve  at: 
45°          60°          70° 
8.833      3.247       1.929  g.  Ce2(SO4)3. 

80°          90°         100.5°  bpt.  of  sat.  solution. 
1.207      0.8355      0.469  g.  Ce2(SO4)3. 

Muthmann  and  Rolig's  determinations  are 
inaccurate.  (Koppel.) 

+8H20.  100  pts.  H2O  dissolve  14.92  pts. 
Ce2(SO4)3  at  20°  from  Ce2(SO4)3+8H2O3 
(John.) 

100  pts.  H2O  dissolve  pts.  Ce2(SO4)3  at  t°. 


t 

Pts. 
Ce2(S04)3 

t 

Pts. 
Ce2(SO4)  3 

0 
18 
30 

19.10 
17.32 
16.13 

50 
60 
70 

12.48 
9.40 
4.24 

(Muthmann  and  Rolig.) 

100  g.  H2O  dissolve  at: 

0°  15°         20.4° 

10.09      11.06      9.525  g.  Ce2(SO4)3, 

30°        40°          50°          60° 
7.388       5.947      4.785      4.064  g.  Ce2(SO4)3. 
Previous    determinations    are   inaccurate. 
(Koppel,  Z.  anorg.  1904,  41.  395.) 

100  g.  sat.  solution  at  25°  contain  7.60  g. 
anhydrous  salt.    (Wirth,  Z.  anorg.  76.  174.) 

Solubility  in  H2SO4+Aq  at  25°.    Solid  phase 

Ce2(SO4)3+8H2O. 


Normality 
H2SO4 

In  100  g.  of  the  liquid  are  dissolved 

g.  Ce2O3 

g.  Ce2(SO4)3 

0 
0.1 
1.1 
2.16 
4.32 
6.685 
9.68 
15.15 

4.604 
4.615 
3.64 
3.01 
2.0 
0.9115 
0.4339 
0.145 

7.60 
7.618 
6.00 
5.018 
3.301 
1.505 
0.733 
0.239 

(Wirth,  Z.  anorg.  1912,  76.  191.) 

+9H2O.    100  pts.  H2O  dissolve  17.52  pts. 
Ce2(SO4)3  from  Ce2(SO4)3+9H2O.    (Brauner. 

100  g.  H2O  dissolve  at: 
0°        15°      21°      30°      31.2° 
20.98   11.87  9.725  7.353  7.185  g.  Ce2(SO4)3, 

31.6°     45°       50°       60°       65° 

7.164    5.13    4.673    3.88    3.595  g.  Ce2(SO4)3. 

(Koppel.)  . 
+  12H2O. 
100  pts.  H2O  dissolve  pts.  Ce2(SO4)3  at  t°. 


0 
18 
25 


Pts.  Ce2(S04)s 


21.40 
18.44 
16.22 


(Muthmann  and  Rolig,  Z.  anorg.  1898,  16. 

457.) 

100  g.  H2O  dissolve  at: 
0°          18.8°       19.2° 
16.56      17.52      17.70  g.  Ce2(S04)3. 
Previous    determinations    are    inaccurate. 
(Koppel.) 

Ceroceric  sulphate,  Ce2(SO4)3,  2Ce(SO4)2-f 
24H2O. 

Decomp.  by  H2O.  Sol.  in  HCl+Aq  with 
decomp.  (Mendelejeff,  A.  168.  45.) 

Ce2(SO4)3,  3Ce(SO4)2+31H2O.    (Jolin.) 

Ceric  sulphate,  basic,  CeO2,  SO3-f  2H2O. 

Very  si.  sol.  in  H2O. 

Sol.  in  2500  pts.  H2O.    (Mosander.) 

Boiling  H20  gradually  dissolves  out  H2SO4. 
(Erk.) 

Sol.  in  acids. 

8CeO2,   7SO3+12H2O;  8CeO2,  7SO3  + 
15H2O;  6CeO2,  5SO3+5H2O;  4CeO2,  3SO3  + 
7H2O;  and  3Ce(SO4)2,  5Ce(OH)4.     All  are 
insol.  ppts. 

Ceric  sulphate,  Ce(SO4)2. 

Anhydrous.  Very  slowly  sol.  in.  cold,  more 
rapidly  in  hot  H2O.  When  solution  has  once 
begun,  almost  unlimited  quantities  may  be 
dissolved.  Insol.  in  cone.  H2SO4.  (Meyer, 
B.  1904,  37.  144.) 

+4H2O.  Sol.  in  H2O  with  immediate  de- 
comp. (Rammelsberg.) 

Decomp.  by  H2O.  (Muthmann,  B.  1900, 
33.  1764.) 

Cerous  hydrogen  sulphate,  Ce2(S04)3,  3H2SO4. 

Decomp.  by  H2O.    (Wyrouboff,  Bull.  Soc. 

(3)  2.  745;  Brauner,  Z.  anorg.  1904,  38.  329.) 

Ceroceric  hydrogen  sulphate,  Ce2H(SO4)4  + 
13H2O. 

Sol.  in  H2O.  Forms  very  supersat.  solu- 
tions. 

Solubility  in  H2SO4  decreases  with  increase 
in  concentration  of  the  acid.  (Meyer,  B. 
1904,  37.  146.) 


SULPHATE,  CHROMIC  HYDROGEN 


957 


Cerous  potassium  sulphate,  Ce2(SO4)3,  K2SO4 
+2H20 

SI.  sol.  in  H2O;  insol.  in  sat.  K2SO4+Aq. 
(Czudnowicz,  J.  pr.  80.  26.) 

2Ce2(SO4)3,  3K2SO4.  As  above.  (Her- 
mann, J.  pr.  30.  188.) 

+8H2O.    (Barre,  A.  ch.  1911,  (8)  24.  249.) 

Ce2(SO4)3,  2K2SO4+3H2O.  As  above. 
(Jolin.) 

Ce2(SO4)3,  3K2SO4.  Sol.  in  about  56  pts. 
H2O  at  9-20°.  Easily  sol.  in  acidified  H2O. 
Nearly  insol.  in  sat.  K2SO4-f  Aq.  (Jolin.) 

Ce2(SO4)3,  5K2SO4.  Insol.  in  K2SO4+Aq. 
(Barre,  J.c.) 

Ceric  potassium  sulphate,  Ce(SO4)2,  2K2SO4 

+2H20. 

SI.  sol.  in  H2O  with  decomp.  Insol.  in  sat. 
K2S04+Aq. 

Ceric  silver  sulphate,  10Ce(SO4)2,  6Ag2SO4. 

Only  si.  sol.  in  cold  H2O;  decomp.  by  hot 
H2O  in  which  it  is  readily  sol.  (Pozzi-Escot, 
C.  R.  1913,  166.  1074.)  ' 

Cerous  sodium  sulphate,  Ce2(SO4)3,  Na2SO4  + 
2H2O. 

Very  si.  sol.  in  H2O,  and  still  less  in  Na2SO4 
+Aq.  100  ccm.  sat.  Na2SO4+Aq  dissolve  an 
amount  corresponding  to  6.2  mg.  Ce2O3. 
(Jolin.) 

SI.  sol.  in  HCl+Aq.    (Czudnowicz.) 

Cerous  thallous  sulphate,  Ce2(S04)3,  3T12SO4. 

Ppt. 

Ce2(S04)3,  T12S04+2H20.  Sol.  in  H2O. 
(Zschiesche,  J.  pr.  107.  98.) 

+4H2O.  Very  si.  sol.  in  cold,  somewhat 
more  in  warm  H2O.  (Wyrouboff,  Bull.  Soc. 
Min.  14.  83.) 

Cerous    tin    (stannic)    hydrogen    sulphate. 

CeHSn(S04)4. 

Decomp.  by  H2O.  Sol.  in  very  dil.  HC1. 
(Weinland,  Z.  anorg.  1907,  64.  251.) 

Chromous  sulphate,  CrSO4+7H2O. 

100  pts.  H2O  dissolve  12.35  pts.  CrSO4+ 
7H2O.  Aqueous  solution  can  be  boiled  with- 
out decomp.  SI.  sol.  in  alcohol. 

+H2O.    (Moissan,  Bull.  Soc.  37.  296.) 

Chromic  sulphate,  basic,  3Cr2O3,  2SO3  + 
12H2O  =2Cr2(SO4)(OH)4,  Cr2(OH)6+ 
5H2O. 

Insol.  in  H2O.  Sol.  in  acids.  Slowly  de- 
comp. by  KOH+Aq  or  K2CO3+Aq. 

5Cr2O3,  3SO3.  Sol.  in  H2O.  (Recoura,  C. 
R.  112.  1439.) 

Cr2O3,  SO3  =  Cr2O2(SO4).  Ppt.  (Schiff,  A. 
124.  167.) 

+10H2O  or  [Cr(OH)2(OH2)4]2SO4.  Nearly 
insol.  in  H2O.  (Werner,  B.  1908,  41.  3451.) 

5Cr2O3,  8SO3  (?).    (Siewert,  A.  126.  97.) 

Cr2O3,  2SO3  =  Cr2O(SO4)2.  Easily  sol.  in  a 
little  H2O,  but  a  precipitate  is  thrown  down 


by  further  addition  of  H2O,  which  redissolves 
on  evaporation. 

5Cr2O3,  12SO3  (?).    (Siewert.) 

2Cr203,  5SO3+15H2O.  Sol.  in  H2O;  insol. 
in  alcohol  and  acetone  by  which  it  is  ppt. 
from  aqueous  solution.  (Nicolardot,  C.  R. 
1907,  146.  1338.) 

Chromic  sulphate,  Cr2(SO4)3. 

Anhydrous.  Insol.  in  H2O.  HNO3,  HC1, 
H2SO4,  aqua  regia,  and  NH4OH+Aq.  De- 
comp. by  boiling  caustic  alkalies,  and 'slowly 
by  alkali  carbonates +Aq.  (Schrotter.)  Ac- 
cording to  Traube  (A.  71.  92)  and  Siewert  (A. 
126.  94),  Schrotter's  salt  is  an  acid  sulphate, 
Cr4(S04)6(OS02OH)2  =  2Cr2(SO4)3,  H2SO4. 
According  to  fitard  (Bull.  Soc.  (2)  31.  200) 
both  salts  exist,  and  formula  of  above  salt  is 
Cr2(SO4)6Cr2.  Formula  is  2[(Cr2O3)2,  (SO3)6], 
17H2SO4  (?).  (Cross  and  Higgins,  Chem. 
Soc.  41.  113.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann. 
B.  1910,  43.  314.) 

+6H2O  (?).  Green  modification.  Readily 
sol.  in  H2O  or  alcohol.  Sol.  in  cone.  H2SO4. 
H2O  solution  is  converted  into  the  violet  mod- 
ification by  standing  3-4  weeks.  (Schrotter.) 

+11H2O  (?).  Extremely  deliquescent;  be- 
comes liquid  in  moist  air  in  2  minutes.  Not 
pptd.  by  BaCl2+Aq.  (Recoura,  C.  R.  113. 
857.) 

+18H2O.  Violet  modification.  Sol.  in 
0.833  pt.  H2O  at  20°.  When  the  H2O  solution 
is  heated  to  65-70°  it  begins  to  be  converted 
into  the  green  modification.  This  conversion 
is  also  brought  about  by  cold  HNO3,  H2SO4, 
PC13.  (fitard,  C.  R.  84.  1090.) 

Sp.  gr.  of  aqueous  solution  of  violet  modi- 
fication of  Cr2(SO4)3  containing: 

5  10  20%  Cr2(SO4)3+18H2O, 

1.0275  1.0560  1.1150 

30  40  50%Cr2(SO4)3+18H2O. 

1.1785      1.2480      1.3250 

Sp.  gr.  of  aqueous  solution  of  green  modi- 
fication of  Cr2(SO4)3  containing: 

10  20  30%Cr2(SO4)3+18H2O, 

1.0510  1.1070  1.1680 

40  50  60%Cr2(S04)3+18H20, 

1.2340      1.3055      1.3825 

70  80%  Cr2(SO4)3+18HO2. 

1.4650       1.5535 

(Gerlach,  Z.  anal.  28.  494.) 

See  also  Chromosulphuric  acid. 

Chromic  hydrogen  sulphate,  Cr2(SO4)3,  H2SO4 

+16H2O. 
Two  modifications. 

a.  Violet.    Decomp.  by  H2O. 

b.  Green.     Obtained  from  violet  modifica- 
tion on  heating.     Sol.  in  H20.     (Weinland, 
Z.  anorg.  1906,  49.  157.) 


958 


SULPHATE,  CHROMIC  CUPRIC 


+24H2O.  Decomp.  by  alcohol,  giving  the 
normal  sulphate.  (Weinland.) 

Cr2(S04)3,  2H2SO4+18H2O.  Hygroscopic. 
Decomp.  by  H2O.  (Weinland.) 

2Cr2(S04)3,  H2S04  =  C 

Correct  composition  of  Cr2(SO4)3  (Traube), 
which  see. 
See  also  Chromosulphuric  acid. 

Chromic  cupric  sulphate,  Cr2(S04)2,  2CuS04, 
H2S04. 

Insol.  in  H2O,  but  gradually  decomp.  there- 
by. (Etard,  C.  R.  87.  602.)  * 

Cr2O3,  CuO,  4SO3. 

Insol.  in  H2O.  (Recoura,  C.  R.  1893,  117. 
39.) 

Chromous  hydrazine  sulphate,  CrSO4,  2N2H4, 

H2S04. 

Only  si.  sol.  in  H2O.  Sol.  in  acids.  (Traube 
B.  1913,  46.  1507.) 

Chromic  hydroxylamine  sulphate,  Cr2(SO4)3, 

(NH2OH)2SO4+24H2O. 
Sol.  in  H2O.    (Meyeringh.) 

Chromic  iron  (ferrous)  sulphate,  Cr2(SO4)3, 

2FeSO4,  H2SO4+2H2O. 
As  above.    (Etard,  I.e.) 

Chromic   iron    (ferric)    sulphate,   Cr2(S04)3, 

Fe2(S04)3. 

Insol.  in  H2O.    (Etard,  C.  R.  86.  1399.) 
Cr2(S04)3,    Fe2(SO4)3,    H2SO4.      Insol.    in 

H20.    (Etard.) 

Chromic  lithium  sulphate,  Cr2(SO4)3,  3Li2SO4. 
Resembles  the  corresponding  K  salt.    (Wer- 
nicke.) 

Chromic    manganous    sulphate,    Cr2(SO4)3, 

3MnSO4. 
(Etard,  C.  R.  86.  1402.) 

Chromic  manganic  sulphate,  Cr2(SO4)3, 

Mn2(S04)3. 

Insol.  in  H2O.    (Etard,  C.  R.  86.  1399.) 
Cr2(SO4)3.  Mn2(SO4)3,  2H2SO4.     SI.  deli- 
quescent.  Sol.  in  H2O  with  decomp.    (Etard.) 

Chromic  nickel  sulphate,  Cr2(SO4)3,  NiS04, 

2H2SO4+3H2O. 

Insol.  in  H2O,  but  gradually  decomp.  there- 
by. (Etard,  C.  R.  87.  602.) 

Chromous  potassium  sulphate,  CrSO4,  K2SO4 

+6H2O. 

Sol.  in  H2O;  less  sol.  in  alcohol.  (Peligot, 
A.  ch.  (3)  12.  546.) 

Chromic  potassium  sulphate,  K2Cr2(SO4)4. 

Anhydrous,  a.  Sol.  in  H2O  when  not  heated 
over  350°. 


/8.  Insol.  in  cold  H2O  and  cold  acids.  When 
ignited  is  insert,  in  hot  H2O  and  acids,  except 
slightly  in  boiling  cone.  H2SO4.  (Fischer.) 

+2H2O  (?) .  Insol.  in  cold  H2O  or  dil.  acids. 
Sol.  by  long  boiling  with  H2O,  and  more 
quickly  when  HC1  is  added.  (Hertwig.) 

+4H20.  Is  potassium  chromosulphate, 
which  see. 

+24H2O.  Chrome-alum.  Violet  modifica- 
tion. Efflorescent  at  29°.  Sol.  in  6-7  pts. 
cold  H2O.  When  the  H2O  solution  is  heated 
to  60-70°  it  is  partially  decomp.  into  a  green 
modification,  which  is  more  sol.  in  H2O.  The 
green  modification  on  standing  in  H20  solu- 
tion is  very  slowly  converted  back  into  violet 
modification.  The  green  modification  may 
also  be  formed  by  heating  dry  salt  to  100  , 
at  which  temp,  it  melts  in  its  crystal  H2O. 
When  all  crystal  H2O  has  been  expelled  at 
300-350°,  it  still  dissolves  in  hot  H2O,  but 
when  heated  above  350°  it  becomes  insol.  in 
H2O.  (Lowel,  A.  ch.  (3)  44.  313.) 

125.1  g.  anhydrous,  or  243.9  g.  hydrated 
salt,  or  0.441  g.  mols.  anhydrous  salt  are  sol. 
in  1  -1.  H2O  at  25°.  (Locke,  Am.  Ch.  J.  1901, 
26.  175.) 

Melts  in  crystal  H2O  at  89°.  (Tilden, 
Chem.  Soc.  45.  409.) 

Sp.  gr.  of  aqueous  solution  of  violet  modi- 
fication at  15°  containing:" 

5  10  15%  K2Cr2(S04)4+24H20. 

1.02725  1.05500  1.08350 

Sp.  gr.  of  sat.  solution  at  15°  =  1.0985. 

Sp.  gr.  of  aqueous  solution  of  green  modi- 
fication at  15°  containing: 

10  20          30%K2Cr2(SO4)4+24H2O, 

1.050      1.103      1.161 

40  50          60%  K2Cr2(S04)4+24H20, 

1.225       1.295      1.371 

70  80          90%K2Cr2(S04)4+24H20. 

1.453      1.541       1.635 

(Gerlach,  Z.  anal.  28.  497.) 

Sp.  gr.  of  chrome-alum  solutions  at  15° 
containing: 

5  10  15  20  25  %salt, 
1.0174  1.0342  1.0524  1.0746  1.1004 

30  35  40  45  50  %  salt, 
1.1274  1.1572  1.1896  1.2352  1.2894 

55         60         65         70      %  salt. 
1.3704  1.4566  1.5462  1.6362 
(Franz,  J.  pr.  (2)  5.  298.) 

Insol.  in  alcohol. 

3K2SO4,  Cr2(SO4)3.  Insol.  in  H2O,  acids,  or 
dil  alkalies.  Decomp.  by  boiling  with  cone. 
KOH+Aq.  (Wernicke,  Pogg.  159.  576.) 

Chromic  rubidium  sulphate,  Rb2Cr2(S04)4+ 

24H2O. 
Sol.  in  H2O.     (Petersson.) 


SULPHATE,  COBALTOUS 


959 


Solubility  in  H2O. 

Solubility  in  100  pts.  H2O  at  t°,  using  CoSO4+ 

7H2O. 

rp                         G.  anhydrous       G.  mols.  of  anhy- 

salt  per  I.            drous  salt  per  1. 

t 

Pt8. 

t° 

Pts. 

Pts. 

CoSO4 

CoSO4 

t° 

CoSO4 

25°                   25  7                  0  079 

30°                   31.7                  0.0$6 

0 

24.6 

36 

43.5 

72 

65.0 

35°                   41.1                  0.128 

1 

25.0 

37 

44.0 

73 

65.6 

40°                   59.7                  0.181 

2 

25.5 

O/j     f\ 

38 

or* 

44.6 

A  t      O 

74 

*7C 

66.2 

nr*     r> 

Melts  in  crystal  H2O  at  107°. 

4 

26.0 
26.5 

o9 
40 

45.2 
45.8 

75 

76 

66.8 
67.4 

(Locke,  Am.  Ch.  J.  1901,  26.  180.) 

5 
6 

27.0 
27.5 

41 
42 

46.4 
47.0 

77 
78 

68.0 
68.6 

7 

28.0 

43 

47.6 

79 

69.2 

Chromic   sodium   sulphate,   Na2Cr2(SO4)4  + 

8 

28.5 

44 

48.2 

80 

69.8 

10H2O. 

9 

29.0 

45 

48.8 

81 

70.4 

Is  sodium  chromosulphate,  which  see. 
+24H2O.     More  efflorescent  than  K  or 
NH4  salt.     Sol.  in  H2O,  and  properties  re- 
semble the  corresponding  K  salt. 
Cr2(SO4)3,  3Na2SO4.    Resembles  the  corre- 
sponding K  salt. 

10 
11 
12 
13 
14 
15 
16 

29.5 
30.0 
30.5 
31.0 
31.5 
32.0 
32.5 

46 
47 
48 
49 
50 
51 
52 

49.4 
50.0 
50.6 
51.2 
51.8 
52.4 
53.0 

82 
83 
84 
85 
86 
87 
88 

71.0 
71.6 
72.2 

72.8 
73.4 
74.0 
74.6 

17 

33.0 

53 

53.6 

89 

75.2 

Chromic   thallous    sulphate,    Tl2Cr2(SO4)4+ 

18 

33.5 

54 

54.2 

90 

75.9 

24H20. 

19 

34.0 

55 

54.8 

91 

76.6 

0.212  mols.  of  anhydrous  salt  are  sol.  in 
1  1.  H2O  at  25°.    1  1.  H2O  dissolves  104.8  g. 
of  anhydrous  or  163.8  g.  hydrated  salt  at 
25°.     Melts  in  crystal  H2O  at  92°.     (Locke, 
Am.  Ch.  J.  1901,  26.  175.) 

20 
21 
22 
23 
24 

34.5 
35.1 
35.6 
36.2 
36.8 

56 
57 
58 
59 
60 

55.4 
56.0 
56.6 
57.2 

57.8 

92 
93 
94 
95 
96 

.  77.2 
77.9 
78.6 
79.2 
79.9 

25 

37.4 

61 

58.4 

97 

80.6 

26 

38.0 

62 

59.0 

98 

81.3 

Chromic   sulphate   chloride,   Cr2(SO4)2Cl2  + 

27 

38.5 

63 

59.6 

99 

81.9 

2H20. 

28 

39.1 

64 

60.2 

100 

82.6 

Slightly  hydroscopic.    Sol.  inH2O.    (Schiff, 
A.  124.  176.) 

29 
30 

39.6 
40.2 

65 
66 

60.8 
61.4 

101 
102 

83.3 
83.9 

[CrSO4,  5H2O]C1.     Sol.  in  H2O.     (Wein- 
land,  Z.  anorg.  1908,  58.  176.) 

31 
32 
33 

40.7 
41.3 
41.8 

67 
68 
69 

62.0 
62.6 
63.2 

103 
104 
105 

84.6 
85.3 
86.0 

34 

42.4 

70 

63.8 

106 

86.7 

Chromyl  sulphate,  (CrO2)SO4. 

35 

42.9 

71 

64.4 

106.4 

86.9 

Decomp.  by  H2O.    (Pictet  and  Karl,  Bull. 

Soc.  1908,  (4)  3.  1114.) 

(Mulder,  calculated  from  his  own  and  Tob- 

Cobaltous  sulphate,  basic. 

Ppt.    Insol.  in  H2O.     (Berzelius.) 

6CoO,  SO3  +  10H2O.     (Athanasesco,  C.  R. 

103.  271.) 
5CoO,  SO3+4H2O.     Ppt.    Very  si.  sol.  in 

H2O.     (Habermann,  M.  Ch.  5.  432.) 

Cobaltous  sulphate,  CoS04. 
100  pts.  H2O  dissolve  at: 
3°      10°     20°     24°    29° 

26.2  30.5  36.4  38.9   40  pts.  anhydrous  salt, 

35°    44°    50°    60°    70° 

46.3  50.4  55.2  60.4  65.7  pts.  anhydrous  salt. 

(Tobler,  A.  96.  193.) 

100  pts.  H2O  at  11-14°  dissolve  23.88  pts. 
anhydrous  salt.     (v.  Hauer,  J.  pr.  103.  114.) 


ler's  determinations,  Scheik.  Verhandel.  1864. 
68.) 

100  g.  H2O  dissolve  37.8  g.  CoSO4  at  25°. 
(Wagner,  Z.  phys.  Ch.  1910,  71.  430.) 

See  also  +7H2O. 


Sp.  gr.  of  CoSO4+Aq  at  t°.  S  =  pts.  CoSO4  in 
100  pts.  solution;  Si  =  mols.  CoSO4  in  100 
mols.  of  solution. 


S 

Si 

Sp.  gr. 

6.8910 
5.8140 
4.7095 
3.5792 
2.4273 
1.2099 

0.852 
0.711 
0.570 
0.429 
0.288 
0.141 

.0765 
.0641 
.0517 
.0392 
.0263 
1.0131 

(Charpy,  A.  ch.  (6)  29.  26.) 

960 


SULPHATE,  COBALTOCOBALTIC 


Sp.  gr.  of  CoSO4+Aq  at  room  temp,  con- 
taining i 

7.239       14.156      21.167%  CoSO4. 
1.0860       1.1591       1.2398 
(Wagner,  W.  Ann.  1883,  18.  269.) 


Sp.  gr.  of  CoSO4+Aq  at  25°. 

t 

g.  CoS04 

t° 

g.  CoS04 

t° 

g.  CoSO4 

0 
5 
10 

25.53 
28.05 
30.55 

15 
20 
25 

33.045 
36.21 
39.35 

30 
35 

40 

42.26 
45.80 

48.85 

Concentration  of  CoSC>4 
+Aq 

Sp.  gr. 

1-normal 

V2-     " 

V<-     " 

Vs-       " 

1.0750 
1.0383 
1.0193 
1.0110 

(Koppel,  Z.  phys.  Ch.  1905,  52.  395.) 

M.-pt.  of  CoSO4+7H2O  =96-98°.    (Tilden, 
Chem.  Soc.  46.  409.) 

(Wagner,  Z.  phys.  Ch.  1890,  5.  37.) 

100  pts.  sat.  solution  of  CoSO4  and  CuSO4 
contain  22.70  pts.  of  the  two  salts. 

Solubility  of  CoSO4,  7H2O+Na2SO4,  10H2O 
in  H2O  at  t°.  100  g.  H2O  dissolve  grams 
CoSO4  and  grams  Na2SO4. 


t 

grams  CoSCU 

grams  Na2SO4 

0 
5 
10 

21.855 
23.94 
25.41 

10.07 
13.155 
16.665 

(Koppel,  Z.  phys.  Ch.  1905,  52.  396.) 

See  also  under  CoNa2(SO4)2+4H2O. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

HC2H3O2  ppts.  it  completely  from  CoS04  + 
Aq.  (Persoz.) 

100  pts.  absolute  methyl  alcohol  dissolve 
1.04  pts.  CoSO4  at  18°.  (de  Bruyn,  Z.  phys. 
Ch.  10.  784.) 

100  pts.  absolute  methyl  alcohol  dissolve 
54.5  pts.  CoSO4+7H2O  at  18°;  100  pts.  ab- 
solute methyl  alcohol  dissolve  42.8  pts.  CoSO 
+7H2O  at  3°;  100  pts.  93.5%  methyl  alcohol 
dissolve  13.3  pts.  CoSO4+7H2O  at  3°;100 
pts.  50%  methyl  alcohol  dissolve  1.8  pts. 
CoSO4+7H2O  at  3°. 

100  pts.  absolute  ethyl  alcohol  dissolve  2.5 
pts.  CoSO4+7H2O  at  3°.  (de  Bruyn,  Z.  phys. 
Ch.  10.  786.) 

100  g.  solution  in  glycol  contain  2.5  g. 
CoSO4.  (de  Coninck,  Bull.  Ac.  Belg.  1905. 
359.) 

Insol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1370.) 

Insol.  in  ethyl  acetate.  (Naumann,  B, 
1904,  37.  3602.) 

+  H2O.  SI.  sol.  in  cold,  and  only  verv 
slowly  sol.  in  hot  H2O.  (Vortmann,  B.  15, 
1888.) 

+4H2O.  (Frohde,  Arch.  Pharm.  (2)  127. 
92.) 

+6H2O.     (Marignac.) 


+7H2O.     Sol.  in  24  pts.  cold  H2O.     Insol. 
in  alcohol.     (Persoz.) 

Solubility   of   CoSO4+7H2O  in  H2O    at    t°. 
100  g.  H2O  dissolve  grams  CoSO4. 


Cobaltocobaltic  sulphate,  Co2O3,  6CoO,  SO3  + 

15H2O. 

Precipitate.  Insol.  in  boiling  CoSO4+Aq 
or  NH4OH+Aq.  (Gentele,  J.  pr.  69.  130.) 

Cobaltic  sulphate,  Co2(SO4)3+18H2O. 

Sol.  in  H2O  with  immediate  decomp.  and 
liberation  of  O.  Sol.  in  dil.  H2SO4+Aq  with- 
out immediate  decomp.  Sol.  in  cone.  HNO3, 
H2SO4,  or  HC2H3O2+Aq.  (Marshall,  Chem. 
Soc.  59.  760.) 

Cobaltous  cupric  sulphate,  2CoS04,  CuSO4-f 
21H20. 

Easily  sol.  in  H2O.  (v.  Hauer,  Pogg.  125. 
637.) 

+36H2O.    (Liebig.) 

2CoSO4,  2CuSO4,  H2SO4.    (Etard.) 

Cobaltous  cupric  magnesium  potassium  zinc 
sulphate,      CoSO4,      CuSO4,      MgSO4, 
4K2SO4,  ZnSO4+24H2O  (?). 
Sol.  inHsO.    (Vohl.) 

Cobaltous  cupric  potassium  sulphate,  CoSO4, 
CuS04,  2K2SO4+12H2O  (?). 

Sol.  inHaO.    (Vohl.) 

Does  not  exist.  (Aston  and  Pickering, 
Chem.  Soc.  49.  123.) 

Cobaltous  hydrazine   sulphate,  CoH2(SO4)2, 

2N2H4. 

1  pt.  is  sol.  in  305.16  pts.  H2O  at  12°.  Sol. 
in  HNO3  with  decomp.  Insol.  in  HC1. 
(Curtius,  J.  pr.  1894,  (2)  50.  331.) 

Cobaltous  iron  (ferrous)  potassium  sulphate, 

CoSO,,  Fe2SO4,  2K2SO4+12H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 
2CoS04,  2FeSO4,  H2SO4.    (Etard.) 

Cobaltous    magnesium    sulphate,    3CoSO4, 

MgS04+28H2O. 
Easily  sol.  in  H2O.    (Winkelblech.) 


SULPHATE  HYDRAZINE,  COBALTOUS 


961 


Cobaltous   magnesium   potassium   sulphate 

CoS04,  MgS04,  K2S04+12H20. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 
Does  not   exist.     (Aston  and  Pickering 
'Chem.  Soc.  49.  123.) 

Cobaltous   manganous   potassium   sulphate 

CoSO4,  MnS04,  2K2SO4+12H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 

Cobaltous  nickel  potassium  sulphate,  CoS04, 
NiS04,  2K2S04+12H20. 

Sol.  in  H2O.    (Vohl,  A.  94.  57.) 

Does  not  exist.  (Thomson,  Rep.  Brit. 
Assn.  Adv.  Sci.  1877.  209.) 

Cobaltous  potassium  sulphate,  CoSO4,  K2SO< 

+6H2O. 

Less  sol.  in  H2O  than  CoSO4. 
100  pts.  H2O  dissolve  at: 
0°     12°    15°    20°    25° 
19.1  30    32.5  39.4  45.3  pts.  anhydrous  salt, 

30°       35°       40°      49° 
51.9     55.4     64.6     81.3  pts.  anhydrous  salt. 
(Tobler,  A.  96.  126.) 

100  pts.  saturated  solution  contain  at: 
20°       40°       60°       80° 
14        19.5      24.4      31.8  pts.  anhydrous  salt. 
(v.  Uauer,  J.  pr.  74.'  433.) 

1  1.  H2O  dissolves  128.8  g.  anhydrous 
salt  at  25°.  (Locke,  Am.  Ch.  J.  1902, 27. 459.) 

Cobaltic  potassium  sulphate,  K2Co2(SO4)4+ 

24H2O. 

Sol.  in  H2O  with  decomp.  (Marshall, 
Chem.  Soc.  69.  760.) 

Cobaltous  potassium  zinc  sulphate,  CoS04, 

2K2S04,  ZnSO4+12H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 

Cobaltous  rubidium  sulphate,  CoSO4,  Rb2SO4 
+6H2O. 

Sol.  in  H2O.    (Tutton.) 

1  1.  H2O  dissolves  92.8  g.  anhydrous  salt 
at  25°.  (Locke,  Am.  Ch.  J.  1902,  27.  459.) 

Cobaltic  rubidium  sulphate,  Rb2Co2(SO4)2+ 

24H20. 

Decomp.  by  H2O.  Sol.  in  dil.  HC1  and 
;H2SO4.  Decomp.  by  cone.  HC1  or  H2SO4. 


by 
1,J. 


(Howe  and  O'Neal,  J.  Am.  Chem.  Soc.  1898, 
20.  762.) 

Melts  in  crystal  H2O  at  47°.    (Locke,  Am. 
Ch.  J.  1901,  26.  183.) 

Cobaltous  sodium   sulphate,  CoNa2(SO4)2  + 
4H20. 


Solubility  of  CoNa2(SO4)2,  4H2O  in  H2O  at  t°. 
100  g.  H2O  dissolve  grams  CoSO4  and 
grams  Na2SO4. 


t° 

g.  CoSO4 

g.  Na2S04 

20 
25 
30 
35 
40 

26.65 
25.365 
23.13 
22.55 
20.975 

24.91 
23.325 
21.61 
20.85 
20.055 

(Koppel,  Z.  phys.  Ch.  1905,  62.  397.) 

Solubility  of  CoNa2(SO4)2,  4H2O+CoSO4, 
7H2O  in  H2O  at  t°.  100  g.  H2O  dissolve 
grams  CoSO4  and  grams  Na2SO4. 


18.5 

20 

25 


28.61 
29.42 
30.73 


23.82 

23.015 

20.575 


CoSO4 


32.695 
34.065 
35.01 


Na2SO< 


18.17 
15.61 
13.715 


(Koppel,  Z.  phys.  Ch.  1905,  62.  397.) 

Solubility  of  CoNa2(SO4)2,  4H2O+NaSO4, 
10H2O  in  H2O  at  t°.  100  g.  H2O  dissolve 
grams  CoSO4  and  grams  Na2SO4. 


18.5 
20 
25 
30 


g.  CcSO4 


25.50 

23.18 

16.07 

9.20 


25.65 
27.26 
35.18 
43.74 


(Koppel.) 

Solubility  of  CoNa2(SO4),  4H2O+Na2SO4 
(anhydrous)  in  H2O  at  t°.  100  g.  H2O 
dissolve  grams  CoSO4  and  grams  Na2SO4. 


35 
40 


g.  CoS04 


7.204 
7.456 


g.  Na2S04 


50.79 
50.095 


(Koppel.) 
See  also  CoSO4+Na2S04  under  CoSO4. 

Cobaltous  zinc  sulphate. 

Efflorescent.      Decomp.    on    air.      (Link, 
Crell.  Ann.  1790, 1.  32.) 

lobaltous  sulphate  ammonia,  CoS04,  6NH«. 

Sol.  hi  H2O  with  separation  of  ppt.    (Rose, 

'ogg.  20.  152.)    Very  easily  sol.  in  NH4OH+ 


Decomp.  by  alcohol. 

Cobaltous  sulphate  hydrazine,  CoSO4,  3NaH4. 
Insol.  in  H2O.     Decomp.  by  boiling  with 
I2O.    Very  sol.  in  dil.  acids  and  NH4-fAq. 
Franzen,  Z.  anorg.  1908,  60.  272.) 


962 


SULPHATE  HYDROXYLAMINE,  COBALTOUS 


Cobaltous  sulphate  hydroxylamine.   CoSO4, 

NH2OH+2H20. 

Insol.  in  cold;  sol.  in  hot  H2O  with  decomp. 
(Feldt,  B.  1894,  27.  403.) 

Columbium  sulphate. 
Sol.  in  H2O.    (Blomstrand.) 

Cuprous  sulphate,  Cu2SO4. 

Decomp.  by  H2O.  Sol.  in  cone.  HC1,  in 
ammonia  and  si.  sol.  in  glacial  acetic  acid. 
(Recoura,  C.  R.  1909,  148.  1107.) 

Cupric  sulphate,  basic,  lOCuO,  SO3. 

(Pickering,  Chem.  Soc.  1907,  91.  1984.) 

8CuO,  SO3-H2H2O.  Ppt.  (Kane,  A.  ch. 
72.  269.) 

5CuO,  SO3+6H2O.  Ppt.  (Smith,  Phil. 
Mag.  J.  23.  196.) 

4CuO,  SO3+3H2O.  Insol.  in  H2O.  (Rou- 
cher,  J.  Pharm.  (3)  37.  50.) 

Min.  Brochantite.  Sol.  in  acids  and 
NH4OH+Aq. 

+3KH2O.  Insol.  in  H2O.  Easily  sol.  in 
dil.  acids,  even  HC2H3O2+Aq.  SI.  sol.  in 
CuSO4+Aq.  Insol.  in  NaC2H302+Aq.  (Cas- 
selmann,  Z.  anal.  4.  24.) 

+4H2O.  Insol.  in  H20.  (Proust.)  Sol. 
in  (NH4)2SO4+Aq,  and  more  easily  in  NH4C1, 
and  NH4NO3+Aq.  (Lea.) 

1 1.  cold  H2O  dissolves  0.017  g.  (Pickering, 
C.  N.  1883,  47.  182.) 

+5H2O.    Min.  Langite. 

+16H2O.    (Andre,  C.  R.  100.  1138.) 

7CuO,  2SO3+5H2O.    (Reindel,  J.  pr.  100. 

1.) 

+6H2O.  Wholly  insol.  in  cold  or  hot  H2O. 
(Habermann,  M.  Ch.  5.  432.) 

+7H2O.  Insol.  in  H2O;  easily  sol.  in  acids. 
Insol.  in  boiling  CuSO4+Aq.  (Reindel.) 

3CuO,  SO3 + 1 KH2O .  Insol.  in  H2O ;  easily 
sol.  in  acids.  (Steinmann,  B.  16.  1412.) 

+2H2O.  Insol.  in  H2O;  sol.  in  dil.  H2SO4+ 
Aq.  (Shenstone,  Chem.  Soc.  47.  375.) 

+2^H2O.    (Reindel,  J.  pr.  102.  204.) 

+4H2O.  Insol.  in  H2O.  (Grimbert  and 
Barre,  J.  Pharm.  (5)  21.  414.) 

5CuO,  2SO3+3H2O.  (Wibel,  Dissert. 
1864.) 

HCuO,  4SO3+8H2O.  (Clowes,  C.  N. 
1898,  78.  155.) 

8CuO,  3SO3+10H2O.  (Marchlewski  and 
Sachs,  Z.  anorg.  1892,  1.  405.) 

7CuO,  3SO3+12H2O.  (fitard,  C.  R.  1887, 
104.  1615.) 

5CuO,  2S03+5H2O.  (Sabatier,  Gm.  K. 
6.  1,  839.) 

6H2O.  Min.  Arnimite.  (Weisbach,  J.  B. 
1886.  2253.) 

2CuO,  SO3.  Decomp.  by  cold  H2O  into 
Cu'SO4  and  4CuO,  SO3.  (Roucher.) 

Insol.  in  H2O.  Decomp.  by  hot  H20. 
,Sol.  in  dil.  acids.  (Pozzi-Escot,  Bull.  Soc. 
.1913  (4)  13.  816.) 

According  to  Pickering  (C.  N.  47.  181)  only 


3CuO,  SO3+23^H2O  and  4CuO,  SO3+4H2O 
are  true  chemical  compounds. 

There  is  at  25°  no  definite  basic  sulphate  of 
copper,  all  the  basic  sulphates  being  solid 
solutions.  The  solutions  in  contact  with 
these  basic  sulphates  contain  S03  and  CuO 
in  equivalent  quantities  and  are  all  si.  acid 
in  reaction.  (Bell,  J.  phys.  Chem.  1908,  12. 
179.) 

Cupric  sulphate,  CuSO4. 

Anhydrous.  Absorbs  H2O  from  the  air. 
Combines  with,  and  dissolves  in  H2O  with 
great  evolution  of  heat. 

+HoO.  Permanent.  Sol.  inH20.  (Etard, 
C.  R.  87.  602.) 

+2H2O  (?).    (Storer's  Diet.) 

+3H2O.    (Etard,  C.  R.  104.  1614.) 

Does  not  exist.    (Cross,  C.  N.  49.  220.) 

See  Foote,  p.  965. 

+5H2O.     Superficially  efflorescent  in  dry 


Sol.  in  2.34  pts.  H2O  at  18°,  and  sat.  solution  has  sp. 
gr.  1.2147.     (Schiflf,  A.  109.  326.) 


100  pts.  CuSO4+Aq  sat.  at  b.  pt.,  102.2°,  contain  45 
pts.  of  the  dry  salt,  or  100  pts.  H2O  at  102.2°  dissolve 
81.82  pts.  CuSO4.  (Griffiths,  Q.  J.  Sci.  18.  90.) 

Sol.  in  less  than  4  pts.  H2O  at  ord.  temp.,  and  much 
more  sol.  in  boiling  H2O.  (Bergmann.) 

Sol.  in  4  pts.  cold,  and  2  pts.  hot  H2O.     (Schubarth.) 

100  pts.  H2O  dissolve  33.103  pts.  CuSO4+5H2O  at 
15°,  and  solution  has  sp.  gr.  =1.1859.  (Michel  and 
Krafft,  A.  ch.  (3)  41.  478.) 

CuSO4+Aq  sat.  at  8°  has  1.17  sp.  gr.     (Anthon,  A. 
24.  210.) 
.    1  pt.  CuSO4+5H2O  dissolves  at:    • 

4°          19°         31°         37.5°         50° 
in  3.32        2.71         1.84  1.7          1.14  pts.  H2O, 


62.5C 
in  1.27 


104°      . 
0.47  pts.  H2O. 
(Brandes  and  Gruner,  1826.) 


75° 
1.07 


87.5° 
0.75 


100° 
0.55 


Sol.  at  17.5  in  2.412  pts.  H2O.      (Karsten.) 

100  pts.  H2CTdissolve  at: 
9°        10°    '  20°      30° 
31.61  36.95  42.31  48.81  pts.  CuSO4+5H2O, 

40°      50°      60°       70° 
56.90  65.83  77.39  94.60  pts.  CuSO4+5H2O, 

80°  90°  100° 

118.03      156.44      203.32  pts.  CuSO4+5H2O 
(Poggiale,  A.  ch.  (3)  8.  463.) 

100  pts.  H2O  dissolve  at: 
0°      20°      35°      54° 
17    24.3     28.6     36.1  pts.  anhydrous  CuS04 
(Tobler,  A.  96.  193.) 

100  pts.  CuSO4+Aq  sat.  at  11-14°  cqntai 
16.23  pts.  anhydrous  CuSO4.  (v.  Hauer,  , 
pr.  103.  114.) 

100  pts.  H2O  dissolve  15.107  pts.  CuSO4 1 
0°.  (Pfaff,  A.  99.  224.) 


SULPHATE,  CUPRIC 


963 


100  pts.  H2O  dissolve  pts.  CuSO4  at  t°. 

If  solubilitv  S  =  pts.  anhydrous  CuSO4  in 
100  pts.  solution,  S  =  11.6+0.2614t  from  -2° 
to  55°;  S  =  26.5+0.3700t  from  55°  to  105°; 
S=45.0.-0.0293t  from  105°  to  190°.    (Etard, 
C.  R.  104.  1614.) 
Solubility  decreases  above  120°,  owing  to 
formation  of  basic  salt.     (Tilden  and  Shen- 
stone,  Phil.  Trans.  1884.  23.) 
100  ccm.  H2O  dissolve  14.92  g.  CuSO4  at  0°. 
(Engel,  C.  B.  102.  113.) 
100  ccm.  H2O  dissolve  22.28-22.30  g.  CuSO4 
at  20°.    (Trevor,  Z.  phys.  Ch.  7.  468.) 

t° 

Pts.  CuSO4 

0 
17.9 
24.1 

14.99 
20.16 
22.37 

(Diacon,  J.  B.  1866.  61.) 

100  pts.  H2O  dissolve  pts.  CuSO4  at  t°. 

100  pts.  H2O  dissolve  pts.  CuSO4  at  t°. 

4-O 

Pts. 

Pts. 

Pts. 

t 

CuSO4 

t° 

CuSO4 

t° 

CuS04 

0 

14.15 

40 

28.50 

80 

54.53 

10 

17.50 

50 

33.31 

90 

64.35 

20 

20.53 

60 

39.01 

100 

75.22 

30 

24.34 

70 

45.74 

(Patrick  and  Aubert,  Transactions  of  Kansas 

Acad.  of  Sci.  1874.  19.) 

Solubility  in  100  pts.  H2O  a-t  t°. 

J.Q 

Pts. 

Pts. 

Pts. 

t 

CuSO4 

t° 

CuSO4 

t° 

CuSO4 

0 

15.5 

35 

27.5 

70 

45.7 

•  1 

16.3 

36 

27.9 

71 

46.4 

2 

16.6 

37 

28.3 

72 

47.2 

3 

16.9 

38 

28.7 

73 

47.9 

4 

17.2 

39 

29.1 

74 

48.7 

5 

17.5 

40 

29.5 

75 

49.5 

6 

17.8 

41 

29.9 

76 

50.3 

7 

18.1 

42 

30.3 

77 

51.1 

8 

18.4 

43 

30.7 

78 

51.9 

9 

18.7 

44 

31.1 

79 

52.7 

10 

19.1 

45 

31.5 

80 

53.5 

11 

19.3 

46 

31.9 

81 

54.3 

12 

19.6 

47 

32.3 

82 

55.1 

13 

19.9 

48 

32.7 

83 

55.9 

14 

20.2 

49 

33.2 

84 

56.8 

15 

20.5 

50 

33.6 

85 

57.8 

16 

20.8 

51 

34.1 

86 

58.7 

17 

21.1 

52 

34.5 

87 

59.7 

18 

21.4 

53 

35.0 

88 

60.7 

19 

21.7 

54 

35.5 

89 

61.7 

20 

22.0 

55 

36.0 

90 

62.7 

21 

22.3 

56 

36.6 

91 

63.7 

22 

22.6 

57 

37.2 

92 

64.8 

23 

23.0 

58 

37.8 

93 

65.8 

24 

23.3 

59 

38.4 

94 

66.9 

25 

23.7 

60 

39.0 

95 

68.0 

26 

24.0 

61 

39.6 

96 

69.1 

27 

24.4 

62 

40.2 

97 

70.2 

28 

•  24.7 

63 

40.9 

98 

71.3 

29 

25.1 

64 

41.5 

99 

72.4 

30 

25.5 

65 

42.2 

100 

73.5 

31 

25.9 

66 

42.9 

101 

74.6 

32 

26.3 

67 

43.6 

102 

75.7 

33 

26.7 

68 

44.3 

103 

76.8 

34 

27.1 

69 

45.0 

104 

77.95 

(Mulder,  Scheik.  Verhandel.  1864.  79.) 

Sat.  CuSO4  +  Aq  contains  %  CuSO4  at  t°. 


t° 

%  CuSO4 

t° 

%  CuS04 

—1 

12.1 

88 

38.8 

+7 

14.1 

89 

38.9 

9 

14.5 

94 

41.8 

18 

16.9 

96 

41.9 

20 

17.2 

97 

42.0 

20 

17.4 

100 

43.6 

35 

21.3 

108 

43.8 

39 

21.8 

110 

43.4 

45 

23.9 

116 

43.8 

54 

26.9 

116 

44.0 

54 

26.6 

120 

44.8 

61 

28.8 

132 

44.8 

63 

29.1 

133 

44.7 

65 

30.0 

143 

45.0 

70 

31.6 

160 

44.2 

71.7 

32.6 

165 

44.5 

76 

34.5 

179 

42.9 

80 

36.6 

189 

42.2 

86 

37.8 

(Etard,  A.  ch.  1894,  (7)  2.  554.) 


Solubility  in  H2O  at  t°. 


t 

g.  CuSO4  per  100  g.  H2O 

0 
10 
15 
20 
25 

14.15 
17.68 
19.25 
20.78 
22.29  (by  interpolation) 

(Cohen,  Z.  phys.  Ch.  1907,  60.  713.) 


1.399  mol.  are  sol.  in  1  1.  H2O  at  25°. 
(Herz,  Z.  anorg.  1910,  67.  366.) 

100  g.  CuS04+Aq  sat.  at  30°  contain  20.32 
anhyd.  CuSO4.  (Schreinemakers,  Z.  phys. 
Ch.  1910,  71.  110.) 

+7H2O.     (Boisbaudran,  C.  R.  66.  1249.) 

+6H2O.    (Boisbaudran,  C.  R.  66.  487.) 


964 


SULPHATE,  CUPRIC 


Sp.  gr.     of 


CuSO4+Aq     at 
CuSO4+5H2O. 


18°.     % 


% 

Sp.  gr. 

% 

Sp.  gr. 

% 

Sp.  gr. 

1 

.0063 

11 

1.0716 

21 

1  .  1427 

2 

.0126 

12 

1.0785 

22 

1.1501 

3 

.0190 

13 

1.0854 

23 

1  .  1585 

4 

.0254 

14 

.0923 

24 

1  .  1659 

5 

.0319 

15 

.0993 

25 

1.1738 

6 

.0384 

16 

.1063 

26 

1.1817 

7 

.0450 

17 

.1135 

27 

1  .  1898 

8 

.0516 

18 

.1208 

28 

1  .  1980 

9 

.0582 

19 

.1281 

29 

1.2063 

10 

.0649 

20 

.1354 

30 

1.2146 

(Schiff,  calculated  by  Gerlach,  Z.  anal.  8.  288.) 


Sp.  gr.  of  CuSO4+Aq  at  23.9°.  a  =  no.  of  Y2 
•mols.  in  grms.  dissolved  in  1000  grms. 
H2O;  b  =  sp.  gr.  if  a  is  CuSO4  =  5H2O  (Y2 
mol.  wt.  =  125);  c  =  sp.  gr.  if  a  is  CuSO4 
(3/2mol.  wt.=80). 


a 

b 

c 

1 
2 
3 

1.076 
1.142 
1.200 

1.080 
1.154 
1.225 

(Favre  and  Valson,  C.  R.  79.  968.) 


Sp.  gr.  of  CuSO4+Aq  at  15°. 

%  =  %CuS04+5H20. 


% 

Sp.  gr. 

% 

Sp.  gr. 

5 

1.0335 

20 

1  .  1443 

10 

1.0688 

25 

1  .  1848 

15 

1  .  1060 

mother 
liquor 

1.185 

(Gerlach,  Dingl.  181.  131.) 


Sp.  gr.  of  CuSO4+Aq  at  18C 


%  CuSO4 

Sp.  gr. 

%  CuSO4. 

Sp.  gr. 

5 
10 

1.0513 
1  .  1073 

15 
17.5 

1  .  1675 
1.2003 

(Kohlrausch,  W.  Ann.  1879.  1.) 


Sp.  gr.  of  CuSO4+Aq  at  0°.    S=pts.  CuSO4 
in  100  pts.  solution. 


s 

Sp.  gr. 

S 

Sp.  gr. 

11.9315 
9.8159 

7.5474 

1.1371 
1.1108 
1.0833 

5.2181 
2.6460 

1.0578 
1.0290 

(Charpy,  A.  ch.  (6)  29.  26.) 


>.  gr.  of  CuSO4+Aq  at  room  temp. 


%  CuSO4 

Sp.  gr. 

6.79 
12.57 
17.49 

1.055 
1.1151 
1.1635 

(Wagner,  W.  Ann.  1883,  18.  265.) 


'   Sp.  gr.  of  CuSO4+Aq  at  25°. 


Concentration  of  Cu  SC>4 
.     +Aq 


1-normal 

Vr-      " 
Vr-      " 

Vr-      " 


Sp.  gr. 


1.0790 
1.0402 
1.0205 
1.0103 
1.0050 


(Wagner,  Z.  phys.  Ch.  1890,  6.  38.) 


B.-pt.  CuSO4+Aq  containing  pts.  CuSO4  to 
100  pts.  H2O. 


B.-pt. 

Pts.  CuSO4 

B.-pt. 

Pts.  CuSCU 

100.5° 

21.3 

103.0° 

69.0' 

101.0 

36.9 

103  .  5 

74.9 

101.5 

48.0 

104.0 

80.1 

102.0 

56.2 

104.2 

82.2 

102.5 

63.0 

(Gerlach,  Z.  anal.  26.  434.) 


Sat.  CuSO4+Aq  boils  at  102.2°,  and  con- 
tains 81.8  pts.  CuSO4  to  100  pts.  H2O. 
(Griffiths.) 

Crust  forms  at  102.3°,  and  solution  contains 
60.3  pts.  CuSO4  to  100  pts.  H2O;  highest  temp, 
observed,  104.8°.  (Gerlach,  Z,  anal.  26.  426.) 

Sol.  in  HCl+Aq,  causing  a^  reduction  of 
temperature  of  about  17°. 

Very  si.  sol.  in  cone.  H2SO4.    (Schulz.) 


Solubility  in  H2SO4+Aq  at  0°. 


G.  per  100  g.  H2O 

Sp.  gr. 

H2SO4 

CuS04 

0.00 

14.85 

1.144 

2.03 

14.29 

1.143 

7.16 

15.65 

1.158 

15.20 

9.90 

1.170 

26.57 

6.43 

1.195 

27.57 

6.19 

1.211 

35.2 

3.99 

1.224 

(Engel,  C.  R.  1887,  104.  507.) 


SULPHATE,  CUPRIC 


965 


Solubility  in  H2SO4+Aq  at  25°. 

Solubility  of  CuSO4  in  CuCl2+Aq  at  30°. 

Solution 

Solid  phase 

%  CuCh 

%  CuSO4 

Solid  phase 

Sp.  gr. 

%  CuO 

%  S03 

0 
6.58 
15.68 
25.67 
39.48 
42.47 
43.25 
43.95 

20.32 
13.62 
8.93 
4.77 
3.21 
2.90 
1.14 
0 

CuS04,  5H20 

it 

ee 

1C 

CuSO4,  5H2O+CuCl2,  2H2O 
CuCl2,  2H2O 

(C 

.2142 

.2248 
.2593 
.2934 
.4061 
.4256 

i;4249 
1.4516 
1.4915 
1.5124 
1.5408 
1.5643 
1.6824 
1.7752 
1.8118 
1.8266 

9.17 
5.91 
3.39 
1.82 
1.32 

1.38 
1.02 

0^38 
0.368 
0.109 
0.105 
0.15 
0.07 

9.26 
15.90 
23.09 
28.75 
39.74 
41.29 

41.04 
43.63 
47.82 
49.07 
51.46 
53.51 
62.14 
68.34 
72  .41 
74.26 

CuSO4  +5H2O 

CuS04+5H2Oand 
CuSO4+3H*O 

CuS04+3H2O 

C.uSO4+H2O 
CuSO4 

(Schreinemakers,  Arch.  Ne'er.  Sci.  1910,   (2) 
15.  117.) 

Solubility  of  CuSO4  in  LiCl+Aq  at  25°. 
Solid  phase,  CuSO4,  5H2O. 
(G.  mols.  per  1.  of  solution.) 

LiCl 

CuSO4 

0 

0.73 
1.40 
2.83 

1.399 
1.257 
1.176 
1.067 

These  results  show  that  the  hydrates  of 
CuSO4  which  are  stable  at  25°  are  CuSO4+ 
5H2O,+3H2Oand+H2O. 

(Bell  and  Taber,  J.  phys.  Chem.  1908,  12. 
175.) 

(Herz,  Z.  anorg.  1910,  67.  366.) 

Solubility  in  H2SO4+Aq  at  25°. 

Solubility  of  CuS04  in  KCl+Aq  at  25°. 
Solid  phase,  CuSO4+5H2O. 
(G.  mols.  per  1.  of  solution.) 

Solution  contains 

Solid  phase 

%  CuSO 

%  H2SO4 

KCl 

CuSOi 

18.47 

12.62 
5.92 
3.25 
2.63 
2.59 
2.83 
2.83 
2.84 
2.70 
2.19 
2.11 
2.15 
0.95 
0.17 
0.15 
0.19 
0.44 
0.42 
0.40 
0.19 

none 
11.14 
25.53 
36.77 
42.15 
47.66 
49.00 
49.20 
49.29 
50.23 
54.78 
55.84 
55.60 
61.79 
77.93 
83.29 
85.46 
85.72 
85.81 
86.04 
92.70 

CuSO4+5H2O 

1     CuSO4+5H2O  and 
CuSO4+3H2O 

CuSO4+3H2O 
UCuS4O4+H2Oan< 
CuSO4+H2O 

CuSO4+H2O  and 
CuSO4 

CuSO4 

0.56 
1.17 
2.34 

1.496 
1.561 
1.819 

(Herz.) 

Solubility  of  CuS04  in  NaCl+Aq  at  25°. 
Solid  phase,  CuS04+5H2O. 
(G.  mols.  per  1.  of  solution.) 

NaCl 

CuSOi 

0 
0.36 
1.32 
2.53 

1.399 
1.404 
1.426 
1.507 

(Herz.) 

These  results  show  that  the  hydrates  of 
CuSO4  which  are  stable  at  25°  are  CuSO4  + 
5H2O,+3H2O  and+H2O. 
(Foote,  J.  Am.  Chem.  Soc.  1915,  37.  290.) 

SI.  sol.  in  sat.  NH4Cl+Aq,  with  separation 
of  a  double  sulphate. 


Solubility  of  CuS04  in  RbCl+Aq  at  25°, 
containing  1.094  g.  mols.  per  1.  =  1.568  g. 
mols.  (Herz.) 

Slowly  sol.  in  sat.  KNO3+Aq,  with  sep- 
aration of  a  double  sulphate. 

Very  slowly  sol.  in  sat.  NaNO3-f  Aq,  with 
separation  of  a  double  sulphate.  (Karsten, 
Berl.  Abhandl.  1840.  10.) 


966 


SULPHATE,  CUPRIC 


Solubility  of  CuSO4  in  (NH4)2SO4+Aq  at  Oc 


g.  per  100  cc. 

g.  par  100  cc. 

so 

ution 

solution 

6 

6 

Sp.  gr. 

g 

. 

Sp.  gr. 

^-N 

GO 

^-v 

02 

i 
fc 

P 

B 

o 

0 

14.79 

1.144 

5.59 

5.13 

1.081 

3.61 

16.09 

1.190 

7.51 

2.95 

1.071 

4.63 

8.38 

1.108 

12.31 

0.94 

1.082 

4.90 

7.26 

1.099 

20.65 

0.80 

1.116 

(Engel,  C.  R.  1886,  102.  114.) 
See  also  under  (NH4)2SO4. 
Solubility  of  CuSO4  in  Li2SO4+Aq  at  30C 


Composition  of  the 

solution 

. 

%  by  wt. 

%  by  wt. 

feoiid  phase 

CuSO4 

Li2S04 

20.32 

0 

CuSO4,  5H2O 

17.50 

3.54. 

ft 

16.10 

6.08 

u 

13.55 

11.94 

(C 

12.14 

15.72 

ft 

11.04 

17.92 

it 

10.05 

20.55 

CuSO4,  5H2O+Li2SO4,  H2O 

10.08 

20.51 

ii 

10.07 

20.49 

<< 

6.41 

22.23 

Li2SO4,  H2O 

3.39 

23.59 

it 

0 

25.24 

u 

(Schreinemakers,  Z.  phys.  Ch.  1909,  66.  692.) 

Sol.  in  CuCl2,  (NH4)2S04,  NH4Cl+Aq  at 
30°.  (Schreinemakers,  Z.  phys.  Ch.  1909,  69. 
565.) 

Sol.  in  (NH4)2SO4,  Li2SO4+Aq.  at  30°. 
(Schreinemakers,  Z.  phys.  Ch.  1909,  66.  694.) 

100  pts.  sat.  solution  of  CuSO4  and  FeSO4 
contain  17.43  pts.  of  the  salts  at  11-14.° 
(v.  Hauer,  J.  pr.  103.  114.) 

100  pts.  H2O  dissolye  10.85  pts.  CuSO4, 
17.47  pts.  MgSO4,  and  5.78  pts.  Na2SO4  at  0°. 
(Diacon.) 

100  pts.  H2O  dissolve  7.169  pts.  CuSO4, 
21.319  pts.  MgSO4,  and  6.330  pts.  Na2SO4  at 
0°.  (Plaff.) 

Slowly  and  si.  sol.  in  sat.  MgSO4+Aq. 
(Karsten.) 

Solubility  of  CuSO4  in  H2O  in  presence  of 
MgSO4.    100  pts.  H2O  dissolve— 


No. 

CuS04 

MgS04 

No. 

5 

6 

7 

CuS04 

MgSO4 

1 

2 
3 
4 

0 
2.64 
4.75 
9.01 

26.37 
25.91 
25.30 
23.54 

12.03 
13.61 
14.99 

15.67 
8.64 
0 

In  1,  2,  and  3,  MgSO4  was  in  excess  and  given 
amt.  CuSO4  added;  in  4,  both  CuSO4  and 


MgSO4  were  in  excess;  in  5,  6,  and  7,  CuSO4 
was  in  excess.  (Diacon,  /.  c.) 

100  pts.  sat.  solution  of  CuSO4  and  MgSO4 
contain  28.58  pts.  of  the  salts  at  11-14°. 
(v.  Hauer,  J.  pr.  103.  114.) 

100  .pts .  sat.  solution'of  CuSO4  and  MnSO4 
contain  37.90  pts.  of  the  salts  at  11-14.° 
(v.  Hauer.) 

Solubility  of  CuSO4+MnSO4  in  H2O  at  25°. 


G.  per  100  g.  H2O 


20.2 
19.76 
13.65 
11.61 


MnS04 


0 

3.69 
31.52 
39.41 


G.  per  100  g.  H2O 


CuS04 


9.39 
6.47 
3.01 
0.0 


MnSO< 


46.77 
53.39 
58.93 
61.83 


(Stortenbecker,  Z.  phys.  Ch.  1900,  34.  112.) 

100  pts.  sat.  solution  of  CuSO4  and  NiSO4 
contain  31.03  pts.  of  the  salts  at  11-14.° 
(v.  Hauer.) 

Solubility  of  CuSO4+NiSO4  in  H2O. 


g.  per  100  g.  H2O 

Mol.  %  CuSCh 

t° 

CuS04 

NiS04 

Solution 

Solid 
phase 

35 

9.62 

583.9 

1.57 

0.35 

41.66 

484.4 

7.69 

2.12 

75.39 

553.5 

11.66 

4.77 

106.40 

506.5 

16.92 

6.52 

172.0 

483.8 

25.6 

13.88 

186.9 

468.8 

27.90 

/18.77 
\94.91 

67 

20.04 

729.3 

2.65 

0.93 

66.01 

706.2 

8.31 

2.86 

88.08 

501.6 

13.55 

3.92 

147.94 

675.0 

16.39 

6.66 

249.9 

747.8 

24.46 

23.32 

(Fock,  Z.  Kryst.  Min.  1897,  28.  387.) 

More  easily  sol.  in  sat.  K2SO4+Aq  than  in 
Na2SO4  or  MgSO4+Aq,  forming  a  double 
sulphate,  which  separates  out.  (Karsten.) 

K2SO4  and  CuSO4  mutually  displace  each 
other  in  saturated  solutions.  (Riidorff,  Pogg. 
148.  555.) 

When  K2S04  and  CuSO4,  both  in  excess, 
are  dissolved  in  H20,  a  maximum  of  solubilitj 
of  15.61  pts.  of  the  two  salts  in  100  pts.  H2C 
at  25°  is  reached  in  30  minutes,  after  whicl 
the  solubility  decreases.  This  result  is  ob 
tained  either  by  treating  excess  of  the  tw< 
salts  with  H2O  at  25°,  or  cooling  solution 
of  the  two  salts  sat.  at  higher  temp,  to  25e 
The  salts  are  in  the  proportion  of  5.2  pts 
K2SO4  to  10.4  pts.  CuSO4.  If  present  in  th 
same  proportion  as  in  their  saturated  soli; 
tions,  5.41  pts.  K2SO4  to  10.13  pts.  CuSC 
would  be  required. 


SULPHATE,  CUPRIC 


967 


If  sat.  solution  of  one  salt  is  added  to  sat. 
solution  of  the  other,  K2Cu(S04)2+6H2O 
separates,  as  it  is  less  sol.  than  either  simple 
salt,  until  a  state  of  equilibrium  is  reached, 
after  which  there  is  no  separation,  contrary  to 
Riidorff  (see  above).  (Trevor,  Z.  phys. 
Ch.  7.  486.) 

CuSO4+Na2SO4. 

Solubility  of  CuSO4  in  presence  of  Na2SO4 
at  0°.    100  pts.  H2O  dissolve— 


No. 

1 
2 
3 

4 

CuSO4 

Na2S04 

No. 

CuS04 

Na.804 

0 
6.01 
9.81 
16.67 

4.53 
5.34 
5.73 
6.48 

5 

6 

7 

15.84 
15.33 
14.99 

3.55 
1.98 
0 

In  1,  2,  and  3.  Na2SO4  was  in  excess  and 
given  amt.  CuS04  added;  in  4,  both  CuSO4 
and  Na2SO4  were  in  excess;  in  5,  6,  and  7, 
CuSO4  was  in  excess  and  Na2SO4  added. 
(Diacon,  J.  B.  1866.  61.) 

100  pts.  H2O  dissolve  8.038  pts.  CuSO4  and 
6.31  pts.  Na2SO4  at  0°.  (Pfaff,  A.  99.  224.) 

100  pts.  H20  dissolve  20.7  pts.  CuSO4  and 
15.9  pts.  Na2SO4  at  15°.  (Riidorff,  B.  6.  484.) 

Solubility  of  CuSO4+Na2SO4. 

1.  Solid    phase,    3    mol.    CuSO4+l    mol. 
Na2SO4.      • 

2.  Solid    phase,    1    mol.    CuSO4+l    mol. 
Na2S04. 

3.  Solid    phase,    1    mol.    CuSO4+3    mol. 
Na2SO4. 

(G.  in  100  g.  H20.) 


t° 

i 

o 

3 

CuSOi 

Na2S04 

CuS04 

Na2S04 

CuSO4 

Na2S04 

12.55 
15.92 
22.70 
15.25 

10 
15 
30 
50 

19.75 
20.69 
22.03 
32.37 

12.49 

15.88- 
16.36 
11.75 

19.70 
20.75 
21.00 
31.45 

12.50 
15.90 
20.14 
13.41 

19.69 
20.70 
15.28 
28.76 

(Massol  and  Maldes,  C.  R.  1901,  133.  287.) 
Solubility  of  CuSO4,  5H2O+Na2SO4,  10H2O. 

t° 

%  CuS04 

%  NaiSOi 

0 
12 
15 

13.40 
14.83 
15.00 

6.23 

9.82 

(Koppel,  Z.  phys.  Ch.  1903,  42.  8.) 
See  also  under  CuNa2(SO4)2+6H2O. 

CuSO4+ZnSO4. 

Very  slowly  sol.  in  sat.  ZnSO4+Aq,  form- 
ing a  double  salt  which  separates.  (Karsten.) 

100  pts.  sat.  solution  of  CuSO4  and  ZnSO4 
contain  .32.70  pts.  of  the  salts  at  11-14°. 
hr.  Hauer.) 


Solubility  of  CuSO4+ZnSO4  in  H2O  at  25C 


Mols.  per  100 

Mols.  per  100 

mols.  H2O 

mols.  H2O 

Cu 

Zn 

Cu 

Zn 

2.28 

0 

0.82 

5.03 

1.83 

2.08 

0.51 

5.59 

1.41 

3.60 

0.30 

5.56 

1.19 

5.01 

0.00 

6.42 

1.86 

3.36 

1.19 

5.01 

1.22 

4.45 

0.51 

5.59 

1.01 

4.72 

0.267 

5.77 

0.00 

5.94 

(Stortenbecker,  Z.  phys.  Ch.  1897,  22.  62.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  827.) 

Insol.  in  liquid  CO2.  (Biichner,  Z.-  phys. 
Ch.  1906,  54.  674.) 

100  pts.  of  a  sat.  solution  in  40%  alcohol 
contains  0.25  pt.  CuSO4+5H2O;  20%  alcohol, 
3.1  pts.;  10%  alcohol,  13.3  pts.  (Schiff,  A. 
118.  362.) 

Anhydrous  CuSO4  is  sol.  in  absolute 
methyl  alcohol,  but  insol.  in  absolute  ethyl 
alcohol.  CuSO4+:rH2O  is  insol.  in  methyl 
or  ethyl  alcohol.  (Klepl,  J.  pr.  (2)  25.  526.) 

100  "pts.  absolute  methyl  alcohol  dissolve 
1.05  pts.  anhydrous  QuSO4  at  18°. 

100  pts.  absolute  methyl  alcohol  dissolve 
15.6  pts.  CuSO4+5H2O  at  18°;  100  pts. 
93.5%  methyl  alcohol  dissolve  0.93  pt. 
CuSO4+5H2O  at  18°;  100  pts.  50%  methyl 
alcohol  dissolve  0.4  pt.  CuSO4+5H2O  at 
18°;  100  pts.  absolute  methyl  alcohol  dis- 
solve 13.4  pts.  CuSO4+5H2O  at  3°. 

100  pts.  absolute  ethyl  alcohol  dissolve  1.1 
pts.  CuSO4+5H2O  at  3°.  (de  Bruyn,  Z. 


phys.  Ch.  10.  786.) 
Me 


ethyl  alcohol  dissolves  11.5%  CuS04-f 
5H2O  at  0°.  (Auger,  C.  R.  1906,  142.  1272.) 

Glacial  acetic  acid  precipitates  CuSO4  com- 
pletely from  CuSO4+Aq. 

100  g.  95%  formic  acid  dissolve  0.05  g. 
CuS04+5H2O  at  18.5°.  (Aschan,  Ch.  Ztg. 
1913,  37.  1117.) 

Sol.  in  glycerine  (Pelouze),  picoline  (Unver- 
dorben). 

100  g.  glycerine  dissolve  36.3  g.  CuSO4-f 
5H2O  at  15-16°.  (Ossendowski,  Pharm.  J. 
1907,  79.  575.) 

100  g.  glycerine  dissolve  30.0  g.  CuSO4  at 
15.5°. 

100  g.  solution  of  CuSO4  in  glycol  contain 
7.6  g.  at  14.6°.  (de  Coninck,  Bull.  Ac.  Belg. 
1905.  257.) 

Anhydrous  CuSO4  is  insol.  in  acetone. 
(Krug  and  M'Elroy,  J.  Anal.  Ch.  6.  184.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014);  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1910,  43.  314);  benzonitrile.  (Naumann, 
B.  1914,  47.  1370.) 

Min.  Chalcanthite. 


968 


SULPHATE,  CUPRIC  GLUCINUM 


Cupric  glucinum  sulphate,  CuSO4,  4GlSO4-f 
20H2O. 

Sol.  hi  H2O.    (Klatzo,  J.  B.  1868.  205.) 

Does  not  exist.  (Marignac,  A.  ch.  (4)  30. 
45.) 

9CuSO4,    G1SO4+50H2O.      As  above. 

Does  not  exist.    (Marignac,  I.  c.) 

Cupric  hydrazine  sulphate,  CuH2(SO4)2, 
2N2H4. 

1  pt.  is  sol.  in  1148  pts.  H20  at  10°. 

Decomp.  by  acids. 

Sol.  in  JSiH4OH+Aq  with  decomp.  (Cur- 
tius,  J.  pr.  1894,  (2)  50.  331.) 

Cupric  iron  (ferrous)  sulphate,  CuSO4,  FeSO4. 

Insol.  in  H2O.    (Etard,  C.  R.  87.  602.) 

+2H2O.    (fitard.) 

CuSO4,  2FeSO4+21H2O.  Sol.  in  H2O.  (v. 
Hauer.) 

CuSO4,  3FeSO4+28H20.  100  pts.  H2O  dis- 
solve 75  pts.  salt  at  7°.  (Lefort.) 

4CuS04,  FeSO4+34H2O.  100  pts.  H2O  at 
15.5°  dissolve  75.91  pts.  (Thomson.) 

Cupric  iron  (ferric)  sulphate,  CuSO4,  Fe2(S04)3 

+24H20. 
Sol.  in  H2O.    (Bastick.) 

Cupric  iron    (ferrous)'    potassium   sulphate, 

CuSO4  FeSO4,  2K2SO4+12H2O. 
Sol.  inH20.    (Vohl.) 

Cupric  lead  sulphate,  CuO,  PbO,  SO8+H2O. 

Min.  Linarite. 

3CuO,  7PbO,  5SO3+5H2O.  Min.  Caledon- 
ite.  Sol.  in  HNO3+Aq. 

Cupric  magnesium  sulphate,  CuSO4,  MgSO4 
+14H2O. 

Efflorescent.  Sol.  in  H2O.  (Vohl,  A.  94. 
57.) 

+2H2O.    (Arrot,  1834.) 

CuSO4,2MgSO4+21H2O.  Sol.inH2O.  (v. 
Hauer,  Pogg.  125.  638.) 

CuSO4,  7MgSO4+56H2O.  Sol.  in  H2O. 
(Schiff,  A.  107.  64.) 

Cupric    magnesium    manganous    potassium 
sulphate,     CuSO4,      MgSO4,      MnSO4, 
3K2S04+18H20. 
Sol.  inH2O.    (Vohl.) 

Cupric  magnesium  potassium  sulphate, 

CuS04,  MgS04,  2K2S04+6H20. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 
Does   not   exist.      (Aston   and    Pickering, 
Chem.  Soc.  49.  123.) 

Cupric  magnesium  potassium  zinc  sulphate, 

CuSO4,  MgO4,  3K2SO4,  ZnSO4+18H2O. 
Sol.  inH2O.    (Vohl.) 


Cupric   manganous    sulphate,    5CuS04, 

2MnSO4+35H2O. 

Sol.  in  H2O.  (Schauffele,  J.  B.  1852.  340.) 
2CuSO4,3MnSO4+25H2O.  As  above.  (S.) 
CuSO4,  MnSO4+H2O.  (Etard,  C.  R.  87. 

602.) 

Cupric  manganous  potassium  sulphate, 

CuSO4,  MnSO4,  2K2SO4+12H2O. 
Sol.  inH2O.    (Vohl.) 

Cupric  nickel  sulphate,  CuS04,  NiSO4+3H2O. 

(Etard,  C.  R.  87.  602.) 

CuSO4,  2NiSO4+21H20.  Sol.  in  H2O. 
(v.  Hauer.) 

+  18H2O.  Sol.  in  H2O.  (Boisbaudran,  C. 
R.  66.  497.) 

2CuSO4,  2NiSO4,  3H2SO4.    (Etard.) 

Cupric  nickel  potassium  sulphate,  CuSO4, 
NiSO4,  2K2SO4-f  12H2O. 

Sol.  in  H2O.    (Vohl.) 

Sol.  in  4  pts.  H2O;  insol.  in  alcohol.    (Bette.) 

4CuSO4,  K2SO4+4H2O.  Very  si.  sol.  in 
H2O. 

K2O,  4CuO,  4SO3+4H2O.  Insol.  in  H2O, 
but  decomp.  by  boiling  H2O  into  3CuO,  SO3. 


Cupric    potassium    sulphate,    K2Cu(S04)2-f- 
6H2O. 

100  pts.  H20  dissolve  66.666  pts.  at  102.8°.  (Grif- 
fiths.) 

Much  more  sol.  in  hot  than  cold  H2O.     (Pierre.) 
Easily  sol.  in  EUO;  by  bailing,  de  comp.  into  basic  salt. 
(Perscz,  A.  ch.  (3)  25.  272.) 

100  pts.  H2O  dissolve  11.14  pts.  anhydrous 
salt  at  25°.  (Trevor,  Z.  phys.  Ch.  7.  470.) 

1  1.  H2O  dissolves  116.9  g.  anhydrous 
salt  at  25°.  (Locke,  Am.  Ch.  J.  1902,  27. 
459.) 

See  also  CuSO4+K2SO4. 

Min.  Cyanochroite. 


Cupric  potassium  zinc  sulphate,  CuSO4, 

2K2SO4,  ZnSO4+12H2O. 
Sol.  in  H20.    (Vohl.) 

Cupric  rubidium  sulphate,  CuSO4.  Rb2SO4+ 
6H20. 

Sol.  in  H2O.    (Tutton.) 

1  1.  H2O  dissolves  102.8  g.  anhydrous 
salt  at  25°.  (Locke,  Am.  Ch.  J.  1902,  27. 
459.) 

Cupric  sodium  sulphate,  basic,  Na2S04, 
Cu(OH)2,  3CuSO4+2H2O. 

Min.  Natrochalcite. 

SI.  sol.  in  H2O;  easily  sol.  in  acids.    (Pa- 
lache  and  Warren,  Am.  J.  Sci.  1908,  (4)  26. 
346.) 


SULPHATE  CARBON  OXIDE,  CUPROUS 


969 


Cupric  sodium   sulphate,  CuSO4,  Na2SO4  + 
2H2O. 

Solubility   of  the  pure  double  salt  CuSO4, 
Na2SO4+2H2O. 


t° 

100  grams  solution  contain 

CuSO4  grams 

Na2SO4  grams 

17.7 
19.5 
23 
30 
40.15 

14.34 
14.54 
14.36 
14.07 
13.73 

13.34 
12.90 
12.76 
12.37 
12.26 

(Koppel.  Z.  phys.  Ch.  1903,  42.  8.) 

Solubility  of  the  mixture  of  CuS04,  Na2SO4  + 
H2O  and  CuSO4. 


t 

100  g.  solution  contain 

CuSO4  grams 

Na2§O4  grams 

17.7 
19.5 
23 
30 
40.15 

14.99 
15.62 
16.41 
17.97 
20.56 

13.48? 
12.06 
11.35 
9.95 
8.00 

(Koppel.) 

Solubility  of  the  mixture  of  CuSO4,  Na2SO4+ 
2H2O  and  Na2SO4. 


t° 

100  g.  solution  contain 

CuSCh  grams 

NaeSCh  grams 

18 

13.53 

13.844 

19.5 

11.847 

15.116 

20 

11.339 

15.697 

23 

8.185 

18.723 

25 

6.284 

21.198 

26 

5.507 

22.44 

28 

3.746 

24.963 

28.3 

3.661 

30 

2.607 

28^383 

30.2 

2.422 

32.2 

1.465 

32^442 

33.9 

1.475 

32.299 

35.3 

1.471 

32.072 

37.2 

1.494 

31.96 

(Koppel.) 

Solubility     of     CuSO4,     Na2SO4+2H2O     in 
presence  of  varying  amounts  of  Na2SO4. 


100  g.  solution  contain 

t° 

CuSO4  grams 

Na2SO4  grams 

30 

5.38 

22.17 

30 

5.41 

21.92 

30.1 

3.69 

25.37 

40.15 

3.97 

23.90 

30 

1.57 

32.09 

(Koppel.) 


Copper  sulphate  and  sodium  sulphate  unite 
to  form  a  double  salt,  CuSO4,  Na2SO4+ 
2H2O,  which  is  stable  in  the  presence  of  the 
solution  above  16.7°.  In  the  presence  of 
copper  sulphate  the  solubility  of  Na2S04+ 
10H2O  is  greater  than  that  of  the  pure  salt. 
(Koppel.) 

Cupric  thalloiis  sulphate,  CuSO4,  T12SO4+ 
6H20. 

Decomp.  by  recrystallising  from  H2O. 
(Willm,  A.  ch.  (4)  6.  55.) 

1  1.  H2O  dissolves  81  g.  anhydrous  salt 
at  25°.  (Locke,  Am.  Ch.  J.  1902,  27.  459.) 

Cupric  zinc  sulphate,  CuSO4,  3ZnS04+28H2O 
Efflorescent.    100  pts.  H2O  dissolve  80  pts. 

salt  at  8°.    Sol.  in  all  proportions  in  boiling 

H2O.     (Lefort.) 

CuSO4,     2ZnSO4+21H2O.       (v.     Hauer, 

Pogg.  125.  637.) 

CuSO*    ZnSO4+12H2O.      (Boisbaudran.) 
2CuSO4,  2ZnSO4,  H2SO4.     (fitard.) 

Cuprous  sulphate  ammonia,  Cu2SO4,  4NH3. 

Sol.  in  NH4OH+Aq;  decomp.  by  pure  H2O. 
(Pochard,  C.  R.  1903,  136.  504.) 

+H2O.  Decomp.  by  H2O.  (Foerster  and 
Blankenburg,  B.  1906,  39.  4434.) 

Cupric    sulphate    ammonia,    basic,    CuSO4, 

3CuO,  2NH3+5H2O. 

Decomp.  by  hot  H2O.  (Pickering,  Chem. 
Soc.  43.  336.) 

Cupric  sulphate  ammonia  (Cuprammonium 
sulphate),  CuSO4,  NH3. 

Decomp.  by  H2O.     (Kane.) 

Decomp.  by  H2O  giving  a  basic  sulphate. 
(Bouzat,  C.  R.  1902, 135.  535.) 

CuSO4,  2NH3  [CuSO4,  2NH3+3H2O. 
(Mendelejeff,  B.  3.  422.)].  Decomp.  by  ex- 
cess of  H2O  into — 

CuSO4,  4NH3+H2O.  Sol.  in  1.5  pts.  H2O, 
but  decomp.  by  much  H2O.  Insol.  in  alco- 
hol. Insol.  in  cone.  NH4OH+Aq.  (Andre*, 
C.  R.  100.  1138.) 

Sol.  in  small  quantity  of  H2O;  decomp.  in 
dil.  solution.  (Bouzat.) 

100  g.  H2O  dissolve  44.56  g.  anhydrous 
comp.  at  25°.  (Pudschies,  Dissert.) 

100  g.  H2O  dissolve  18.05  g.  at  21-22°. 
(Horn  and  Taylor,  Am.  Ch.  J.  1904,  32.  268.) 

CuSO4,  5NH3.  Completely  sol.  in  H2O. 
(Rose,  Pogg.  20.  150.) 

Sol.  in  small  amt.  of  H2O;  decomp.  in  dil. 
solution.  Insol.  in  liquid  NH3.  (Bouzat, 
C.  R.  1902,  135.  535.) 

Cuprous  sulphate  carbon  monoxide,  Cu2SO4, 

2CO+H20. 

Very  unstable.  (Joannis,  C.  R.  1903,  136. 
615.) 


970 


SULPHATE  ZINC  OXIDE,  CUPRIC 


Cupric  sulphate  zinc  oxide,  CuSO4,  2ZnO  + 

21H20. 

(Larsen,  Ch.  Z.  Report.  1896,  20.  317.) 
2CuSO4,  3ZnO+12H2O.     (Mailhe,  A.  ch. 

1902,  (7)  27.  169.) 

Didymium  sulphate,  basic,  Di2O3,  SO3  = 
(DiO)2SO4. 

Insol.  in  cold  or  boiling  H2O.     (Marignac.) 

Slowly  sol.  in  hot  dil.  HCl+Aq.  Easily  sol. 
in  cone,  acids. 

+8H2O.     Precipitate.      (Hermann.). 

Composition  is  2Di2O3/,  3SO3+3H2O  or 
Di2(SO4)3+Di2O6H6.  (Frerichs  and  Smith.) 

Composition  is  5Di2O3,  3SO3+xH2O. 
(Cleve,  B.  11.  910.) 

Didymium  sulphate,  Di2(SO4)3. 

Anhydrous.     By  saturating  cold  H2O  and 
warming  the  solution,  the  following  results 
were  obtained — 100  pts.  H2O  dissolve  at: 
12°      18°      25°      38°      50° 
43.1    25.8   20.6    13.0    11.0  pts.  Di2(S04)3. 

+6H2O.  H2O  dissolves  this  salt  very 
slowly;  100  pts.  H2O  dissolve  13  pts.  Di2(SO4)3 
in  24  hours,  and  16.4  pts.  in  2  days.  If 
solution  is  evap.  in  vacuo  until  Di2(SO4)3  + 
8H2O  separates  out,  34  pts.  Di2(SO4)3 
remain  dissolved  in  100  pts.  H2O. 

+5H2O.    (Cleve.) 

+8H2O.    Solutions  of  this  salt  contain  at: 
19°       40°      50°      100° 

11.7     8.8     6.5     1.6  pts.  Di2(SO4)3. 
(Marignac,  A.  ch.  (3)  38.  170.) 

+9H2O.  (Zschiesche,  J.  Pr.  107.  75.) 

Didymium  potassium  sulphate,  K2S04, 

.  Di2(SO4)3+2H2O. 

Sol.  in  63  pts.  H2O.  Insol.  in  sat.  K2SO4+ 
Aq.  (Marignac.) 

3K2SO4,  Di2(SO4)3.  Sol.  in  83  pts.  H2O  at 
18°.  Insol.  in  cold,  si.  sol.  in  boiling  sat. 
K2SO4+Aq,  100  ccm.  of  which  retain  55  mg. 
Di2O3  in  solution.  (Cleve.) 

4K2SO4,  Di2(SO4)3.    (Cleve.) 

9K2SO4,  2Di2(SO4)3+3H2O.    (Cleve.) 

Didymium    sodium    sulphate,    Di2(S04)8, 

Na2SO4,  and  +2H2O. 
Sol.  in  200  pts.  H2O  (Marignac),  and  still 
less  in  sat.  Na2SO4-f  Aq,  100  ccm.  of  which 
dissolve  only  70  mg.   Di2O3  at  ord.   temp. 
(Cleve.) 

Didymium   thallous    sulphate,    (Di2S04)3, 
3T12SO4. 

Ppt. 

Di2(SO4)3,  T12SO4+2H2O.  Sol.  in  H2O. 
(Zschiesche,  J.  pr.  107.  98.) 

Erbium  sulphate,  Er2(S04)s. 

Anhydrous.  Easily  and  rapidly  sol.  in 
H2O.  100  pts.  H2O  dissolve  43  pts.  anhy- 
drous salt  at  0°. 


N 

C 

Ci 

N 

C 

Ci 

0 
0.1 

1.1 

2.16 

4.604 
4.615 
3.64 
3.04 

7.60 
7.618 
6.00 
5.018 

4.32 
6.685 
9.68 
15.15 

2.00 
0.9115 
0.4439 
0.145 

3.301 
1.505 
0.733 
0.239 

+8H2O.  Less  sol.  in  H2O  than  anhydrous 
salt.  100  pts.  H2O  dissolve  30  pts.  Er2(SO)4)3 
+8H2O  (=23  pts.  Er2(SO4)3)  at  about  20°; 
at  100°,  100  pts.  Er2(SO4)3+8H2O  remain 
dissolved.  Sat.  solution  deposits  crystals 
when  heated  to  55°.  (Hoglund.) 

100  g.  of  sat.  solution  of  Er2(SO4)3+8H2O 
at  25°  in  H2O  contains  11.94  g.  anhyd. 
Er2(SO4)3.  (Wirth,  Z.  anorg.  1912,  76.  174.) 


Solubility  of  Er2(SO4)3+8H2O  in  H2SO4  at 
25°. 

N  =  equiv.  g.  H2SO  in  1  1.  of  solvent. 

C  =  g.  oxide  in  100  g.  of  solution. 

C1  =  g.  anhyd.  salt  in  100  g.  of  solution. 


(Wirth,  Z.  anorg.  1912,  76.  174.) 


Insol.    in    methyl    acetate.      (Naumann, 
B.  1909,  42.  3790.) 


Erbium     potassium      sulphate,     Er2(SO4)3, 

3K2S04. 
Slowly  sol.  in  H2O.     (Hoglund.) 

Erbium  sodium  sulphate,  Er2(S04)3,  5Na2S04 

+7H20. 
Sol.  in  H2O.    (Cleve.) 


Europium  sulphate,  Eu2(SO4)3+8H2O. 

Stable  in  the  air.     (Urbain  and  Lacombe, 
C.  R.  1904,  138.  628.) 

Gadolinium    sulphate,    Gd2(SO4)3+8H2O. 
Solubility  in  H2O. 


Temp. 

Pts.  of  Gd2(SO4)3in 
100  pts.  H2O 

0° 

3.98 

9.3-10.6° 

3.33 

14.0° 

2.80 

25.0° 

2.40 

34.4° 

2.26 

(Benedicks,    Z.    anorg.    1899,    22.    409-410.) 

100  g.  sat.  solution  of  Gd(SO4)3+8H2O 
at  25°  in  H2O  contain  2.981  g.  anhyd. 
Gd2(SO4)3.  (Wirth,  Z.  anorg.  1912,  76.  174.) 


SULPHATE,  GLUCINUM 


971 


Solubility  in  ] 

N  =  equiv. 
C  =  g.  oxide 

C                                 -L 

*2SO4.   Solid  phase,  Gd2(SO4)3  + 
8H20. 
g.  H2SO4  in  1  1.  of  solvent. 
5  in  100  g.  of  solution, 
yd.  Gd2(SO4)3  in  100  g.  of  solu- 

Solubility  of  G1SO4  in  H2SO4+Aq  at  25°. 

H2S04+Aq 
%  H2S04 

100  g.  of  the 
solution  con- 
tain g.  G1SO4 

Solid  phase 

i  —  g.  ann 
tion. 

5.23 
9.61 
18.70 
34.00 
40.35 
45.51 
50.63 
56.59 
63.24 
65.24 
73.64 

8.212 
8.429 
7.944 
6.603 
5.631 
5.773 
6.628 
5.438 
3.640 
2.244 
2.128 
2.185 

1 

}•      G1SO4+6H2O 

G1SO4+4H2O 

J 

X 

c 

Cn 

N 

C 

CM 

0 
0.1 
0.505 
1.1 

1.793 
1.98 
2.365 
2.29 

2.981 
3.291 
3.931 

3.807 

2.16 
6.175 
12.6 

1.789 
0.528 
0.0521 

2.974 

0.8777 
0.0867 

(Wirth.) 
Sol.  in  sat.  K2SO4+Aq. 

Gadolinium  potassium   sulphate,  Gd2(SO4)3, 

K2SO4+2H2O. 

100  grams,  sat.  solution  in  K2SO4+Aq  con- 
tains 0.87 — 0.77  grams  Gd2O3.  (Benedicks, 
Z.  anorg.  1900,  22.  410.) 

Gallium  sulphate,  Ga2(SO4)3. 

Not  deliquescent,  but  very  sol.  in  H2O. 
Sol.  in  60%  alcohol;  insol.  in  ether.  (Bois- 
baudran.) 

Aqueous  solution  decomp.  into  basic  salt 
by  boiling,  which  redissolves,  however,  on 
cooling. 

Gallium  potassium  sulphate,  Ga2K2(S04)4+ 

24H2O. 
(Soret,  Arch.  sc.  phys.  nat.  1885,  14.  96.) 

Gallium   rubidium    sulphate,    Rb2Ga2(S04)4 

+24H2O. 
(Soret,  Arch.  sc.  phys.  nat.  1885,  14.  96.) 

Glucinum  sulphate,  basic,  3G1O,  SO3+4H2O. 

Sol.  in  H2O,  but  decomp.  by  heating  or 
dilution.  (Berzelius.) 

2G10,  SO3+3H2O.    Sol.  in  H20. 

9G1O,  SO3+14H2O  (?).  Precipitate.  In- 
sol. in  H2O.  (Berzelius.) 

Accorolmg  to  Debray,  this  salt  when  care- 
fully washed  is  G1O2H2. 

Glucinum  sulphate,  G1SO4. 

Anhydrous. 

Nearly  insol.  in  H2O,  but  slowly  attacked 
by  cold,  rapidly  by  hot  H2O,  and  is  converted 
into  G1S04+4H2O  before  dissolving.  (Par- 
sons, Z.  anorg.  1904,  42.  253.) 

Sp.  gr.  of  GlSO4+Aq  at  25°. 


Concentration  of  G1SO4 
+Aq 

Sp.  gr. 

1  —  normal 

Vr-     " 

V4—           " 
1/16—          " 

1.0451 
1.0229 
1.0114 
1.0027 

(Wagner,  Z.  phys.  Ch.  1890,  5.  35.) 


(Wirth,  Z.  anorg.  1913,  79.  359.) 
See  also  under  +2,  4,  and  6H2O. 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J., 
1898,  20.  828.) 

+H2O.  (Levi-Malvano,  Z.  anorg.  1906, 
48.  447.) 


+2H2O. 


Solubility  in  H2O  at  t°. 


t° 

G.  G1S04  per  100  g. 

H2O 

Solution 

80 
91.4 
105 

119 

84.76 

97.77 
118.4 
149.3 

45.87 
49.42 
54.21 

59.88 

(Levi-Malvano.) 


+4H2O.     Very  sol.  in  H2O. 

Sol.  in  its  own  weight  of  H20  at  14°,  and 
in  every  proportion  of  boiling  H2O.  Less  sol. 
in  dil.  H2SO4+Aq  than  in  water.  (Debray, 
A.  ch.  (3)  44.  25.) 

Solubility  in  H2O  at  t°. 


g.  G1SO4  per 

g.  G1SO4  per 

t° 

100  g. 

t° 

100  g. 

H20 

solution 

H2O 

solution 

30 

43.78 

30.45 

95.4 

90.63 

47.55 

40 

46.74 

31.85 

107.2 

115.3 

53.58 

68 

61.95 

38.27 

111 

128.3 

56.19 

85 

76.30 

43.28 

( Le  vi-M  al  vano . ) 

SI.  sol.  in  dilute,  insol.  in  absolute  alcohol. 

Can  be  completely  pptd.  from  GlSO4+Aq 
by  HC2H302.  (Persoz.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329.) 


972 


SULPHATE,  GLUCINUM  IRON 


+6H2O. 
Solubility  in  H2O  at  t°. 

Gold   (auric)   sulphate,  Au2O3,   2SO3+H2O, 
or  Auryl  hydrogen  sulphate,  (AuO)HSO4. 
Deliquescent.     Decomp.  by  H2O.    Sol.  in 
HCl+Aq;  not  attacked  by  cone.  HNO3-{- 
Aq.     Sol.  in  6  pts.  cone.  H2SO4.     (Schott- 
lander.) 

Gold  (auric)  potassium  sulphate,  Au2(SO4)8, 
K2SO4. 
Not  decomp.  immediately  by  cold  H2O. 

fS5r>V»r>tflaTirlai«  'i 

t 

g.  G1SO4  per  100  g. 

H2O 

solution 

31 
50 
72.2 

.    77.4 

52.23 
60.67 
74.94 

81.87 

34.32 
37.77 
42.85 
45.01 

(Levi-Malvano . ) 


100  g.  of  the  aqueous  solution  contain  at 
25°,  8.212  g.  G1SO4.  (Wirth,  Z.  anorg.  1913, 
79.358.) 


Glucinum   iron    (ferrous)    sulphate,    G1SO4, 

FeS04+17^H20. 

Sol.  in  H2O.    (Klatzo,  J.  B.  1868.  204.) 
3G1SO4,    FeSO4+28H2O.      Sol.    in    H2O. 

(Klatzo.) 
Do  not  exist.     (Marignac,  A.  ch.  (4)  30. 

45.) 


Glucinum  nickel  sulphate,  (Gl,Ni)SO4+ 
4H2O,  or  7H20. 

(Klatzo,  J.  B.  1868.  205.) 

Does  not  exist.  (Atterberg,  Sv.  V.  A.  F. 
1873,  4.  81.) 


Glucinum  potassium  sulphate,  G1S04,  K2S04 
+2H20. 

SI.  sol.  in  cold,  slowly  but  more  sol.  in  hot 
H2O.  (Debray.) 

+3H2O.     (Klatzo.) 


Glucinum  potassium  hydrogen  sulphate, 

G1H2(SO4)2,  2K2SO4+4H2O. 
Easily  sol.  in  H2O.     Partly  decomp.  by 
recrystallisation.     (Atterberg.) 


Glucinum  sodium  sulphate,  2G1SO4,  3Na2SO4 

+18H2O. 
Sol.  in  H2O.    (Atterberg.) 


Glucuium  zinc  sulphate,  2G1SO4,  3ZnSO4+ 

35H20. 

Sol.  in  H2O.     (Klatzp,  J.  B.  1868.  205.) 
Does  not  exist.     (Atterberg.) 


Gold   (auroauric)   sulphate,  Au2(SO4)2. 

Decomp.  by  moist  air,  H2O,  glacial  acetic 
acid,  or  HNO3+Aq  (1.42  sp.  gr.)  Insol.  in 
cone.  H2SO4.  (Schottlander,  A.  217.  375.) 


Hydrazine  mercuric  sulphate  hydrazine, 

(N2H5)2S04,  3HgS04,  2N2H4. 
Insol.  in  H2O.     Sol.  in  H2O   containing 
HC1.      (Ferratini,   Gazz.   ch.   it.    1912,    42. 
(1)  142.) 


Hydroxylamine  uranyl  sulphate, 

(NH2OH)2,  H2SO4,  2(UO2)SO4+5H20. 
Extremely  sol.  in  H2O  from  which  it  can 
be  cryst.     (Rimbach,  Dissert.  1904.) 

Indium  sulphate,  In2(SO4)3. 
Easily  sol.  in  H20. 
+9H2O.    Easily  sol.  in  H2O. 

Indium    hydrogen    sulphate,     InH(S04)j+ 

4HO.  • 
Very  deliquescent.    (Meyer.) 

Indium  potassium  sulphate,  InK(SO4)2+ 
4H20. 

Sol.  in  H20,  but  decomp.  by  boiling. 
(Rossler,  J.  pr.  (2)  7.  14.) 

(InO)3K(SO4)2+3H2O.  Insol.  in  H20. 
(Rossler.) 

Indium  rubidium  sulphate, 

In2(S04)3,  Rb2S04+24H20. 

44.28  pts.  are  sol.  in  100  pts.  H2O  at  15°. 
(Chabrie-,  C.  R.  1901,  132.  473.) 

Melts  in  crystal  H2O  at  42°.  (Locke, 
Am.  Ch.  J.  1901,  26.  183.) 

Indium  sodium  sulphate,  InNa(SO4)2+4H20. 
Sol.  in  H2O.    (Rossler,,  J.  pr.  (2)  7.  14.) 

Iodine  sulphate,  I2(SO4)3. 

Ppt.  Decomp.  by  H2O.  (Fichter,  Z. 
anorg.  1915,  91.  140.) 

lodyl  sulphate,  (IO)2(SO4)8. 

Possible  composition  of  Weber's  (B.  20. 
86)  I2O6,  3SO3. 


SULPHATE,  IRON 


973 


Iridium  sulphate. 

Solubility  in  100  pts.  H2O  at  t°. 

Sol    in  H2O  or  alcohol      (B6rz6lius.) 

Ir(SO4)2.      Sol.    in   H26.      (Rimbach,    Z 

t° 

Pts. 

t° 

Pts. 

t° 

Pts. 

anorg.  1907,  62.  409.) 

FeSO4 

FeSO4 

FeSO4 

0 

7.9 

34 

37.1 

67 

65.1 

Iridium  potassium  sulphate,  Ir2(SO4)3, 
K2SO4+24H2O. 

1 
2 
3 

8.7 
9.5 
10.4 

35 
36 
37 

38.0 
38.9 
39.8 

68 
69 
70 

65.0 
64.9 
64.8 

Mpt.  102-103°. 

4 

11.2 

38 

40.7 

71 

64.7 

Easily  sol.  in  H2O.     (Marino,  Z.  anorg. 

5 

12.0 

39 

41.7 

72 

64.5 

1904,  42.  220.) 

6 

12.9 

40 

42.6 

73 

64.4 

Ir2(SO4)3,    3K2S04.    Sol.  in  H2O    or    dil. 

7 

13.7 

41 

43.5 

74 

64.2 

H2SO4+Aq;  nearly  insol.  in  sat.    K2SO4+ 

8 

14.5 

42 

44.4 

75 

64.0 

Aq.      (Boisbaudran,   C.   R.  96.  1406.) 

9 

15.3 

43 

45.3 

76 

63.7 

10 

16.2 

44 

46.2 

77 

63.4 

Iridium  rubidium  sulphate,  Ir2(SO4)4Rb2. 

11 

17.0 

45 

47.1 

78 

63.1 

Sol.  in  cold;  very  sol.  in  hot  H2O.    (Marino, 
Gazz.  ch.  it.  1903,  32,  (2)  511.) 
Mpt.  108-109°.    (Marino,  Z.  anorg.  1904, 
42.  219.) 

12 
13 
14 
15 

17.9 
18.7 
19.5 
20.4 

46 

47 
48 
49 

48.1 
49.0 
50.0 
51.0 

79 

80 
81 

82 

62.7 
62.3 
61.9 
61.5 

16 

21.2 

50 

51.9 

83 

61.0 

Iridium  thallium  sulphate,  Ir2(SO4)3,  Tl2SO4-f 

17 
18 

22.1 
23.0 

51 
52 

52.9 
53.8 

84 

85 

60.4 
59.8 

24H2O. 

19 

23.8 

53 

54.8 

86 

59.2 

Very    sol.  in    H2O.      (Marino,    Z.    anorg. 

20 

24.7 

54 

55.7 

87 

58.5 

1904,  42.  222.) 

21 

25.6 

55 

56.7 

88 

57.7 

22 

26.4 

56 

57.7 

89 

57.0 

Iron  (ferrous)  sulphate,  FeSO4. 

23 

27.3 

57 

58.7 

90 

56.2 

+H2O. 

24 

28.1 

58 

59.7 

91    ' 

55.3 

+2H2O.    Not  more  sol.  in  H2Q  than  gyp- 
sum.    (Mitscherlich.) 

25 

26 

29.0 
29.9 

59 
60 

60.7 
61.7 

92 
93 

54.3 
53.3 

+3H2O.    Sol.  in  H2O.    (Kane.) 

27 

30.8 

61 

62.7 

94 

52.2 

+4H2O.    Separates  from  cone.  FeSO4+Aq 
at  80°. 

28 
29 

31.7 
32.6 

62 
63 

63.7 

64.8 

95 
96 

51.0 
49.6 

+7H2O.    Efflorescent  at  33°. 

30 

33.5 

63.5 

65.4 

97 

48.0 

31 

34.4 

64 

65.4 

98 

46.3 

1  pt.  FeSO4+7H2O  dissolves  in  1.6  pts.  cold,  and  0.3 

32 

35.3 

65 

65.3 

99 

44.5 

pt.  boiling  H2O. 
1  pt.  FeSO4+7H2O  dissolves  at: 

33 

36.2 

66 

65.2 

100 

42.6 

10°    15°     25°    33°   46°     60°     8t°    90°  100° 

in  1.64  1.43  0.87  0.66  0.44  0.38  0.37  0.27  0.3  pts.  H2O 
(Brandes  and  Firnhaber,  Br.  Arch.  7.  83.) 

(Mulder,  Scheik.  Verhandel.  1864.  141.) 

When  boiled  with  insufficient  H2O  for  solution  a 
white  hydrate  is  formed  which  separates  out.  Solubility 
increases  up  to  87.5°,  and  then  diminishes,  owing  to  the 
above  separation.  (Brandes,  Pogg.  20.  581.) 

Sol.  in  2  pts.  cold,  and  1  pt.  boiling  H2O  (Fourcroy) : 
sol.  in  2  pt.s  cold  H2O  at  18.75°  (Abl) ;  sol.  in  6  pts.  H2O 
at  moderate  heat,  and  0.75  pt.  at  100°.  (Bergmann.) 

100  pts.  H2O  at  15.5°  dissolve  45-50  pts.  (Ure's 
Diet.) 

100  ftis.  H2O  dissolve  pts.  FeSO4  at  t°. 


t° 

Pts. 
FeS04 

t° 

Pts. 
FeS04 

t° 

Pts. 
FeS04 

o 

10 
12 
20 

15.8 
19.9 
21.3 
28.0 

21 
30 
37 

27.4 
32.6 
36.5 

45 
55 
70 

42.9 
47.0 
56.5 

(Tobler,  A.  95.  198.) 

100  pts.  FeSO4+Aq  sat.  at  11-14°  contain 
17.02%  FeSO4.  (v.  Hauer,  J.  pr.  103.  114.) 

100  pts.  FeSO4+Aq.  sat  at  15°  contain 
37.2%  FeSO4+7H2O;  solution  has  sp.  gr. 
1.2232.  (Schiff,  A.  118.  362.) 


If  solubility  S=pts.  anhydrous  FeSO4  in 
100  pts.  solution,  S  =  13.5+0.3788t  from  —2° 
to  +65°;  S  =  37.5  constant  from  65°  to  98°; 
S  =  37.5— 0.6685t  from  98°  to  156°.  Practi- 
cally insol.  at  156°.  (fitard,  C.  R.  106. 
740.) 

Sat.  FeSO4+Aq  contains  at: 
— 1°       +5°      24°        34°        52° 


1O.U 

60° 

J.O.  JL 

67° 

22.  / 

77° 

2v.«      0^.070  reov/4, 
86°        94° 

36.4 

37.7 

37.8 

37.8      36.7%FeSO4, 

102° 

112° 

130° 

152° 

34.7 

28.0 

17.3 

2.5%FeS04. 

(Etard,  A.  ch.  1894,  (7)  2.  553.) 


100  g.  H2O  dissolve  26.69  g.  FeSO4  at  25°. 
(Stortenbecker,  Z.  phys.  Ch.  1900,  34. 
109.) 


974 


SULPHATE,  IRON 


Solubility  of  FeSO4  in  H2O  at  t°. 
100  g.  H2O  dissolve  g.  FeSO4. 

Sol.  in  hot  HCl+Aq.     (Kane.) 
Somewhat  sol.  in  cone.  H2SO4.    (Bussy  and 
Lecann.) 

Solubility  in  H2SO4+Aq  at  25°. 

t° 

G.  FeSO4 

t° 

G.  FeSO4 

0.00 
10.00 
15.25 
20.13 
25.02 
30.03 
35.07 
40.05 
45.18 
50.21 

15.65 
20.51 
23.86 
26.56 
29.60 
32.93 
36.87 
40.20 
44.32 
48.60 

52.00 
54.03 
60.01 
65.00 
68.02 
70.04 
77.00 
80.41 
85.02 
90.13 

50.20 
52.07 
54.95 
55.59 
52.31 
56.08 
45.90 
43.58 
40.46 
37.27 

H2S04+Aq 
Normality 

100  g.  of  the 
solution 
contain 
g.  FeSO4 

Solid  phase 

0 
2.25 
6.685 
10.2 
12.46 
15.15. 
19.84 

22.84 
19.03 
13.40 
10.30 
7.26 
4.015 
0.1522 

FeSO4+7H2O 

FeSO4+H2O 

J 

FeSO4+7H2O    is    stable  from—  1.82°    to 
+56.6°;  FeSO4+4H2O  from  56.6°  to  64.4°; 
FeSO4+H2O  above  this  point. 
(Fraenckel,  Z.  anorg.  1907,  56.  228.) 

(Wirth,  Z.  anorg.  1913,  79.  364.) 

FeSO4+Aq  sat.  at  30°  contains  24.9  g. 
FeSO4  in  100  g.  of  solution.  (Schreine- 
makers,  Z.  phys.  Ch.  1912,  71.  110.) 

Sp.  gr.  of  FeSO4+Aq  at  15°. 

%  =  %FeSO4+7H2O. 


% 

Sp.  gr. 

% 

Sp.  gr. 

% 

Sp.  gr. 

1 

1.005 

15 

1.082 

28 

1.161 

2 

1.011 

16 

1.088 

29 

1.168 

3 

1.016 

17 

1.094 

30 

1.174 

4 

1.021 

18 

1.100 

31 

1.180 

5 

1.027 

19 

1.106 

32 

1.187 

6 

1:032 

20 

1.112 

33 

.193 

7 

1.037 

21 

1.118 

34 

.200 

8 

.043 

22 

1.125 

35 

.206 

9 

.048 

23 

1.131 

36 

.213 

10 

.054 

24 

1.137 

37 

.219 

11 

.059 

25 

1.143 

38 

.226 

12 

1.065 

26 

1.149 

39 

.232 

13 

1.071 

27 

1.155 

40 

.239 

14 

1.077 

(Gerlach,  Z.  anal.  8.  287.) 

Sp.  gr.  16.6°  of  sat.  solution  =  1.219. 
(Greenish  and  Smith,  Pharm.  J.  1903,  71. 881.) 

Sat.  FeSO4+Aq  boils  at  102.2°  (Griffiths), 
and  solution  contains  64%  FeSO4.  Crust 
forms  at  102.3°;  highest  temp,  observed, 
104.8°.  (Gerlach,  Z.  anal.  26.  426.) 

B.-pt.  of  FeSO4+Aq  containing  pts.  FeSO4 
to  100  pts.  H2O. 


B.-pt. 

Pts.  FeSO4 

B.-pt. 

Pts.  FeSO4 

100.5° 
101.0 

17.7 
34.4 

101.5° 
101.6 

50.4 
53.2 

(Gerlach,  Z.  anal.  26.  433.) 

100  g.  of  the  sat.  solution  contain  22.84  g 
FeSO4  at  25°.  (Wirth,  Z.  anorg.  1913,  79 
364.) 


More  sol.  in  water  containing  NO  than  in 
pure  H2O.  (Gay,  Bull.  Soc.  (2)  44.  175.) 

Completely  pptd.  from  FeSO4+Aq  by 
glacial  HC2H3O2.  (Persoz.) 

Solubility  in  (NH4)2SO4+Aq.  See  under 
(NH4)2S04. 


ooiuiDiiiiy  in  .L*i2ow4-t-/iq  at  ou  . 

Composition  of 
the  solution 

Solid  phase 

% 
by  wt. 
FeSCU 

,% 

by  wt. 
Li2S04 

24.87 
22.45 
21.15 
18.79 
16.51 
16.18 
16.04 
15.39 
12.68 
5.32 
3.74 
0 

0 
4.00 
5.58 
11.16 
15.81 
16.52 
16.49 
16.80 
18.31 
22.15 
23.15 
25.1 

FeSO4,t7H2C 

t{ 
u 

FeSO4,  7H2O+Li2SO4,  H2O 
tt 

Li2SO4,  H2O 
ft 

C( 

(( 

(Schreinemakers,  Z.  phys.  Ch.  1910,  71.  110.) 

Solubility  of  FeSO4,  H2O+Na2SO4,   10H2O4, 
in  100  g.  H2O  at  t°. 

t 

Grams  FeSO4 

Grams  Na2SO4 

0 
15.5 

18.08 

25.05 

6.13 
15.97 

(Koppel,  Z.  phys.  Ch.  1905,  52.  405.) 
See  also  under  FeNa2(SO4)2. 

Insol.  in  liquid  NH3.     (Franklin,  Am.  Ch. 

J.  1898,  20.  828.) 

Insol.  in  liquid  CO2.  (Biichner,  Z.  phys. 
Ch.  1906,  54.  674.) 

100  pts.  sat.  solution  of  FeSO4  in  40% 
alcohol  contains  0.3%  FeSO4.  (Schiff.) 


SULPHATE,  IRON 


975 


Insol.  in  alcohol  of  0.905  sp.  gr.  or  less. 
(Anthon,  J.  pr.  14.  125.) 

Alcohol  and  H2SO4  precipitate  FeSO4  from 
FeSO4+Aq,  also  glacial  acetic  acid. 

Anhydrous  FeSO4  is  insol.  in  acetone. 
(Krug  and  M'Elroy,  1893.) 

Insol.  in  acetone.     (Eidmann,  C.  C.  1899, 

11.  1014.) 

100  g.  sat.  solution  in  gycol  contain  6.0 
g.  FeSO4  at  ord.  temp,  (de  Coninck.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 
B.  1904,  37.  3601.) 

Iron  (ferrous)  sulphate,  acid,  2FeO,  3SO3, 

2H2O. 

This  salt  exists  in  contact  with  solutions 
containing  SO3+1.637  H2O  to  about  SO3  + 
2.186  H2O.  (Kenrick,  J.  phys.  Chem.  1908, 

12.  704.) 

FeO,  2SO3+H2O.  This  compd.  exists  with 
solutions  containing  SO3+ 1.342  H2O  to 
(about)  SO8 +1.595  H2O.  (Kenrick.) 

FeO,  4SO3+3H2O.  This  compd.  is  stable 
with  solutions  containing  from  SO3+ 1.122 
H2O  to  (about)  SO3  +  1.342  H2O.  Rapidly 
sol.  in  H2O  with  ppt.  of  FeSO4+H20.  (Ken- 
rick.) 

Min.  Melanterite. 

Iron  (ferric)  sulphate,  basic,  10Fe2O3,  SO3  + 
H2O. 

(Athanasesco,  C.  R.  103.  27.) 

6Fe2O3,  SO3+10H2O.  Insol.  in  H2O.  SI 
sol.  in  warm  HCl+Aq.  (Scheerer,  Pogg.  45. 
188.) 

4Fe2O3,  SO3+11H2O.  (Anthon,  Repert, 
81.  237.) 

3Fe2O3,  SO3+4H2O.  Insol.  in  H2O, 
Rather  easily  sol.  in  acids.  (Scheerer,  Pogg 
44.  453;  Meister,  B.  8.  771.) 

2Fe2O3,  SO3+6H2O.  When  pptd.  from 
cold  solutions,  is  sol.  in  Fe2(SO4)3+Aq,  but 
insol.  therein  when  pptd.  from  hot  solutions 
(Maus.) 

Only  basic  sulphate  which  is  a  true  chem- 
ical compound.  (Pickering,  Chem.  Soc.  37 
807.) 

Min.  Glockerite.  Insol.  in  H2O.  Sol.  in 
cone.  H2SO4. 

+7H2O.    (Meister.) 

+8H2O.    (Muhlhauser.) 

+  15H2O.    Min.  Pissophanite. 

Fe2O3,  SO3  =  (FeO)2SO4+3H2O.  Insol.  in 
H2O.  (Soubeiran,  A.  ch.  44.  329.) 

3Fe2O3,  4SO3+9H2O.    (Athanasesco.) 

2Fe2O3,  3SO3+8H2O.  Insol.  in  H2O 
(Wittstein.) 

+  18H2O.  Min.  Fibroferrite.  SI.  sol.  in 
cold,  more  easily  in  hot  H2O. 

Fe2O3,  2SO3+10H20.    Min.  Stypticite. 

+15H2O.  Sol.  in  H2O;  decomp.  by  heat 
or  evaporation.  (Muck,  J.  pr.  99.  103.) 

2Fe2O3,  5SO3+13H2O.      Min.   Copiapite. 

Fe4S6O2+18H2O  =2Fe2O3,  5SO3+18H2O 
a-Copiapit.  This  salt  is  in  equilibrium  at  25C 


with  solutions  in  which  the  molecular  ratio 
Fe2O3  :  SO3  lies  between  1  : 2.889  and 
1  : 2.614.  (Wirth,  Z.  anorg.  1914,  87.  37.) 

(OH)Fe3(SO4)4+13H2O.  p-Copiapit.  This 
salt  is  in  equilibrium  at  25°  with  solutions 
in  which  the  molecular  ratio  Fe2O3:SOs  lies 
between  1:3.472  and  1:2.889.  (Wirth,  Z. 
anorg.  1914,  87.  37.) 

According  to  Pickering  (Chem.  Soc.  37. 
807),  all  basic  ferric  sulphates  are  mixtures 
excepting  2Fe2O3,  S03. 

Iron  (ferric)  sulphate,  Fe2(SO4)3. 

Anhydrous.  Slowly  deliquescent.  Nearly 
insol.  in  H2O,  and  HCl+Aq.  Insol.  in  cone. 
H2SO4.  Very  rapidly  sol.  in  FeSO4+Aq,  even 
when  very  dil.  (Barreswil,  C.  R.  20.  1366.) 

Sp.  gr.  of  Fe2(SO4)3+Aq.  According  to  F 
=  Franz  at  17.5°  (J.  pr.  (2)  5.  280);  G  =  Ger- 
lach  at  15°  (Z.  anal.  28.  494);  H  =  Hager  at 
18°  (Z.  anal.  27.  280). 

5          10          15       20  %  Fe2(S04)3, 

F    1.0426  1.0854  1.1324  1.1826 

G      ...  1.096  ...      1.205 

H   1.046  1.097  1.151     1.208 

25          30          35         40  %  Fe2(SO4)3, 

F    1.2426  1.3090  1.3782  1.4506 

G     ...  1.331  . . .  1.478 

H   1.271  1.337  1.411  1.490 

45          50          55          60  %  Fe2(SO4)3. 
F    1.5298   1.6148   1.7050  1.8006 
G     ...        1.650       ...         ... 

Solubility  in  H2SO4+Aq  at  25°. 


H2S04+Aq 
Normality 

100  g.  of  the  solution 
contain  g.  Fe2(SO4)s 

2.25 

6.685 
19.84 

25.02 

14.58 
0.05 

(Wirth,  Z.  anorg.  1913,  79.  364.) 
Solubility  in  Al2(SO4)3+Aq  at  25°. 


100  g.  of  the  solution  contain 


G.  Al2(SO4)s 

G.  Fe2(SO4)a 

44.97 

2.342 

42.44 

5.200 

38.83 

6.626 

35.82 

8.819 

34.02 

10.03 

32.42 

*10.23) 

31.90) 

10.70} 

31.91J 

*Solution  sat.  with  respect  to  both  salts. 
(Wirth  and  Bakke,  Z.  anorg.  1914,  87.  48.) 
See  also  under  A12(SO4)3. 

Insol.  in  liquid  NH3.     (Gore,  Am.  Ch.  J. 
1898,  20.  828.) 


976 


SULPHATE,  IRON 


Completely  pptd.  from  Fe2(SO4)3+Aq  by 
HC2H3O2.  Sol.  to  large  extent  in  alcohol. 

Insol.  in  methyl  acetate.  (Naumann  B. 
1909,  42.  3790);  ethyl  acetate.  (Naumann, 

B.  1910,  43.  314.) 
Insol.  in  acetone. 

+zH2O.  Very  deliquescent,  and  sol.  in 
H2O.  Cone.  Fe2(SO4)3+Aq  may  be  boiled 
without  decomp.,  but  dil.  solutions  are  de- 
comp.  on  heating.  A  solution  containing  1 
pt.  salt  to  100  pts.  H2O  becomes  turbid  at 
76°;  1  pt.  to  200  pts.,  at  56°;  1  pt.  to  400  pts., 
at  47°;  1  pt.  to  800  pts.,  at  40°;  1  pt.  to  1000 
pts.,  at  38°;  1  pt.  to  10,000  pts.,  at  14°. 
(Scheerer.) 

+9H2O.    Min.  Coquimbite. 

81.43  pts.  are  sol.  in  18.57  pts.  H2O. 
(Wirth,  Z.  anorg.  1914,  87.  23.) 

This  salt  is  stable  at  25°  only  in  contact 
with  solutions  in  which  the  molecular  ratio 
Fe2O3  :  SO3  lies  between  1  : 3.472  and  1  : 
6.699.  (Wirth,  Z.  anorg.  1914,  87.  35.) 

+10H2O.  Slowly  sol.  in  H2O.  (Oudemans, 
R.  t.  c.  3.  331.) 

Iron  (ferroferric)  sulphate,  6FeSO4, 

Fe2(SO4)3+60H2O. 
Sol.  in  all  proportions  in  H2O.    (Poumarede. 

C.  R.  18.  854.) 

3FeSO4,  2Fe2(SO4)3  +  12H20.  Decomp.  by 
H20.  Easily  sol.  in  dil.  HCl+Aq.  Insol.  in 
alcohol.  (Abich,  1842.) 

FeSO4,  Fe2(SO4)3+12H2O.  Min.  Voltaite. 
Difficultly  sol.  in  H2O. 

FeO,  Fe2O3,  6SO3+15H2O.  Deliquescent. 
(Lefort,  J.  Pharm.  (4)  10.  87.) 

Iron  (ferrous)  pi/rosulphate,  FeS2O7. 

Deliquescent.  Decomp.  by  H2O.  (Bolas, 
Chem.  Soc.  (2)  12.  212.) 

Iron  (ferric)  hydrogen  sulphate,  Fe2(SO4)3, 
H2SO4+8H2O. 

This  salt  is  in  equilibrium  at  25°  only  with 
solutions  where  the  molecular  ratio  Fe203  : 
SO3  is  more  acid  than  1  :  6.699.  (Wirth  and 
Bakke,  Z.  anorg.  1914,  87.  34.) 

Sat.  solution  of  Fe2(SO4)3,  H2SO4+8H20 
in  abs.  alcohol  at  25°  contains  8  jg.  Fe2O3+ 
17.18  g.  SO3  per  100  g.  sat.  solution.  (Wirth 
and  Bakke.) 

Decomp.  by  H2O.  (Recoura,  C.  R.  1903, 
137.  118.) 

In  contact  with  solutions  containing  25% 
to  28%SO3  at  25°,  the  stable  solid  is  Fe2O3, 
3SO3  -j-  10H2O .  In  contact  with  solutions  con- 
taining more  than  28%,  the  stable  solid  is 
Fe2O3,  4SO3  +  10H2O.  (Cameron  and  Robin- 
son, J.  phys.  Chem.  1907,  11.  650.) 

Iron  (ferroferric)  hydrogen  sulphate, 

Fe2(S04)3,  FeS04,  2H2SO4. 
Insol.  in  H2O,  but  slowly  decomp.  thereby. 
Sol.  inH2S04.    (Etard,  C.R.  87.  602.) 


Iron  ( ferrous)  hydrazine  sulphate,  FeH2(SO4)2» 

2N2H4. 

1  pt.  is  sol.  in  325  pts.  H2O  at  12°.  (Curtius, 
J.  pr.  1894,  (2)  60.  331.) 

Iron  (ferrous)  magnesium  sulphate.  FeSO4> 

MgSO4+4H2O. 
Sol.  inH2O.    (Schiff.) 

Iron  (ferric)  magnesium  sulphate.  Fc2(SO4)8. 
MgS04+24H20. 

(Bastick.) 

Iron  (ferrous)  magnesium  potassium  sulphate. 
^     2K2S04,  FeSO4,  MgS04+12H2O. 
Sol.  in!H2O.    (Vohl,  A.  94.  57.) 

Iron  (ferric)  manganous  hydrogen  sulphate, 
Fe2(SO4)3,  2MnSO4,  H2S04. 

Insol.  in  cold  H2O.    (Etard.) 

Fe2(SO4)3,  2MnS04,  3H2SO4.  Sol.  in  H2O. 
(Etard,  C.  R.  86.  1399.) 

Iron  (ferric)  manganic  sulphate,  Fe2(SO4)3, 

Mn2(S04)3. 

Insol.  in  cold  H2O;  decomp.  by  hot  H2O 
and  HC1  +Aq.  (Etard.) 

Iron  (ferrous)  manganous  potassium  sulphate, 

FeSO4,  MnS04,  2K2SO4+12H2O. 
SoUin  H20.    (Vohl,  A.  94.  57.) 

Iron     (ferrous)     nickel    sulphate,     2FeSO4, 

2NiSO4,  H2SO4. 
(Etard,  C.  R.  87.  602.) 

Iron  (ferric)  nickel  sulphate,  Fe2(SO4)8,  NiS04, 

2H2SO4. 

Insol.  in  H2O,  but  gradually  decomp. 
thereby.  (Etard,  C.  R.  87.  602.) 

Iron    (ferrous)    nickel    potassium    sulphate, 

FeSO4,  NiSO4,  2K2SO4+12H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 

Iron   (ferrous)   potassium   sulphate,   FeSO<, 

K2S04. 
+2H2O.    (Marignac,  Ann.  Min.  (5)  9.  19.) 

Solubility  in  H2O  at  t°. 


t° 

%  FeK2(S04)2 

t° 

%FeK2(S04)2 

0.5 
17.2 
40.1 
60 

22.79 
31.98 
40.86 
42.63 

80 
90 
95 

42.34 
42.73 
41.01 

(Kiister  and  Thiel,  Z.  anorg.  1899,  21.  116.) 

SULPHATE,  IRON  SODIUM 


977 


+4H20. 

G=Gerlach,  at  15°  (Z.  anal.  28.  496);  F  = 

Solubility  in  H2O  at  t°. 

Franz,  at  17.5°  (J.  pr.  (2)  5.  288),  containing: 

5         10      15%  K2Fe2(S04)4+24HaO, 
F   1.0268  1.0466  1.0672 

t° 

%FeK2(S04)2 

t° 

%  FeK2(SO4)2 

0.5 

22.94 

80 

40.46 

G  1.025     1.0507  1.0773 

17.2 
40.1 

26.79 
32.41 

90 
95 

43.82 
44.11 

20         25      30%  K2Fe2(S04)4+24H2O, 
F   1.0894  1.1136  1.1422 

60 

35.68 

G  1.1050  1.1340  1J645 

(Kiister  and  Thiel.) 

+6H20.    100  pts.  H2O  dissolve  at  t°: 
0°     10°  14,5°  16°     25° 
19.6  24.5  29.1  30.9  36.5  pits,  anhydrous  salt, 

35°   40°   55°     65°     70° 
41     45     56    59.3   64.2  pts.  anhydrous  salt. 
(Tobler,  A.  96.  193.) 

Solubility  in  H2O  at  t°. 


t 

%FeK2(SO4)2 

t° 

%  FeK2(SO4)2 

0.5 
17.2 
40.1 

18.36 
25.16 
36.72 

60 
80 

42.93 
45.29 

(Kiister  and  Thiel.) 

Iron  (ferric)  potassium  sulphate,  basic. 
4Fe203,  K20,  7S03+9H20=4(Fe208, 
2H2O,  SO,),  K2S04+7H2O. 

Insol.  in  boiling  H2O.  SI.  sol.  in  HCl+Aq, 
more  readily  in  aqua  regia.  (Rammelsberg.) 

3Fe2O3,  K20, 4SO3+6H2O  =K(FeO)3(S04)2 
+3H2O.  Min.  Jarosite. 

Fe2O3,  H2O,  2SO3,  2K2SO4+5H2O.  Sol.  in 
6  pts.  cold  H2O.  Solution  soon  decomposes. 
(Maus,  Pogg.  11.  78.) 

Sol.  in  12.5  pts.  H2O  at  10°.  (Anthon,  Re- 
pert.  76.  361.) 

Formula  is  given  as  3Fe2O3,  5K2O,  12SO3+ 
18H2O  by  Marignac. 

3Fe2O3,  6SO3,  2K2SO4+22H2O.  Sol.  when 
moist  in  H2O.  Solution  soon  decomposes. 
Insol.  in  alcohol.  (Soubeiran,  A.  ch.  44.  329.) 

3Fe2O3,  7SO3,  5K2SO4+12H2O,  and 
+17H2O.  (Scheerer,  Pogg.  87.  81.) 

2Fe2O3,  5SO3,  3K2SO4+9H2O.    (S.) 

3Fe2O3,  8SO3,  4K2SO4+20H2O  and  24H2O. 
(S.) 

Iron  (ferric)  potassium  sulphate,  K2SO4, 
2Fe2(S04)3. 

Insol.  in  H2O,  but  is  gradually  decomp. 
thereby.  (Grimm  and  Ramdohr,  A.  98.  127.) 

+2H2O.  Nearly  insol.  in  H2O.  (Weinland, 
Z.  anorg.  1913,  84.  364.) 

K2Fe2(SO4)4+24H2O.     Iron  alum. 

Sol.  in  5  pts.  H2O  at  12.5°.    (Anthon.) 

Aqueous  solution  is  decomp.  by  heating. 
Insol.  in  alcohol. 

Sp.  gr.  of  aqueous  solution.    According  to 


35  %  K2Fe2(S04)4+24H20. 
G  1.1967. 


Melts  in  crystal  H2O  at  28°.  (Locke,  Am. 
Ch.  J.  1901,  26.  183.) 

Fe2(SO4)s,,  3K2SO4.  Insol.  in  H2O,  but 
slowly  decomp.  thereby,  (fitard,  C.  R.  84. 
1089.) 

Iron  (ferric)  potassium  sulphate  sulphite. 
See  Sulphite  sulphate,  ferric  potassium. 

Iron  (ferrous)  potassium  zinc  sulphate,  FeS04, 

2K2SO4,  ZnSO4rfl2H2O. 
Sol.  in  H20. 

Iron    (ferrous)    rubidium    sulphate,    FeS04, 

Rb2S04+6H20. 

Sol.  in  H2O.    (Tutton,  Chem.  Soc.  63.  337.) 
1  1.  H2O  dissolves  242  g.  anhydrous    salt 

at  25°.    (Locke,  Am.  Ch.  J.  1902,  27.  459.) 

Iron    (ferric)    rubidium    sulphate,    RbjFei 

(S04)2+24H20. 

Solubility  in  H2O. 


Temp. 

G.  per  litre 

Gram  mols. 
of  anhydrous 
salt  per  litre 

25 
30 
35 

97.4 

202.4 
Basic  salt  formed 

0.294 
0.617 

(Locke,  Am.  Ch.  J.  1901,  26.  180.) 

Iron    (ferrous)    sodium    sulphate,    FeSO4, 

Na2SO4+4H2O. 

Sol.  in  H2O.    (Marignac,  Ann.  Min.  (5)  9. 
25.) 

Solubility  of  FeNa2(SO4)2+4H2O  in  100  g. 
H2O  at  t°. 


t° 

Grams  FeSO4 

Grama  Na!iSO4 

21.8 
24.92 
34.95 
40 

24.34 
23.62 
23.91 
24.01 

22.51 
22.04 
21.83 
22.62 

(Koppel,  Z.  phys.  Ch.  1905,  62.  406.) 


978 


SULPHATE,  IRON  SODIUM,  BASIC 


Solubility      of      FeNa2(SO4)2.4H2O+FeSO4. 
7H2O  in  100  g.  H2O  at  t°. 


t 

grams 
FeSCU 

grams 

Na2SO4 

t° 

grams 
FeS04 

grams 
Na2S04 

18.8 
23 

27 

26.63 

28.82 
30.95 

20.28 
18.40 
16.68 

31° 
35° 

40° 

33.99 
35.66 
39.98 

14.41 
13.85 
11.92 

(Koppel.) 

Solubility     of     FeNa2(SO4)2.4H2O+Na2SO4. 
"10H2O  in  100  g.  H2O  at  t°. 


t° 

grams 
FeS04 

grams 
Na2S04 

t 

grams 
FeS04 

grams 
Na2SO4 

18.8 
23 

27.23 
20.31 

22.16 
26.48 

28° 
31° 

11.28 
6.95 

35.94 
44.75 

(Koppel.) 

Solubility     of     FeNa2(SO4)2.4H2O  +Na2SO4 
(anhydrous)  in  100  g.  H2O  at  t°. 


t° 

grams  FeSO4 

grams  Na2SO4 

46.58 
46.99 

35 

40 

6.16 
6.27 

(Koppel.) 

See  also  under  FeSO4. 
Iron  (ferric)  sodium  sulphate,  basic,  2Na2O, 

Fe2O3,  4SO3+7H2O. 

Only  si.  sol.  in  H2O  with  decomp.  (Skrabal, 
Z.  anorg.  1904,  38.  319.) 

+8H2O.  Min.  Urusite.  Insol.  in  H2O; 
easily  sol.  in  HCl+Aq. 

.  3Na2O,  Fe2O3,  6S03+6H2O.    Sol.  in  H20 
with  decomp.    (Skrabal.) 
4Fe2O3,  Na2O,  5SO3+9H20. 
Insol.  in  H2O;  difficultly  sol.  in  HCl+Aq. 
(Scheerer,  Pogg.  45.  190.) 
Iron  (ferric)  sodium  sulphate,  [Fe(SO4)3]Na3 

+3H2O. 

Ppt.  Nearly  insol.  in  H2O.  (Weinland,  Z. 
anorg.  1913,  84.  365.) 

Iron    (ferrous)    thallium    sulphate,    FeSO4, 

T12SO4+6H20. 

Easily  decomp.  by  solution  in  H2O.  (Willm, 
A.  ch.  (4)  6.  56.) 

Iron  (ferric)  thallium  sulphate,  Tl2Fe2(SO4)4 
+24H2O. 

Not  efflorescent.    Very  easily  sol.  in  H2O. 

361.5  g.  anhydrous,  or  646  g.  hydrated 
salt  are  sol.  in  1  1.  H2O  at  25°,  or  0.799  mol. 
of  the  anhydrous  salt  is  sol.  in  1 1.  H2O  at  25°. 
Melts  in  crystal  H2O  at  37°.  (Locke,  Am. 
Ch.  J.  1901,  26.  175.) 

Iron  (ferrous)  zinc  sulphate,  FeSO4,  ZnS03+ 

14H2O. 

2FeSO4,  2ZnSO4,  H2SO4.  (Etard,  C.  R.  87. 
602.) 

Iron  (ferric)  zinc  sulphate,  Fe2(SO4)3,  ZnSO4 

+24H20. 
(Bastick.) 


Iron  (ferrous)  sulphate  nitric  oxide,  FeSO4, 
NO. 

The  solubility  of  NO  in  FeSO4+Aq  is 
diminished  by  the  presence  of  H2S04,  HC1, 
phosphoric  acid  and  by  the  presence  of  cer- 
tain salts.  (Manchot,  A.  1910,  372.  157.) 

Fe(NO)SO4,  FeSO4+13H2O.  Decomp.  in 
the  air.  Sol.  in  water.  (Manchot.) 

Lanthanum  sulphate,  basic,  2La2O8,  3SOa+ 

3H2O. 

Precipitate.    (Frerichs  and  Smith.) 
Formula  is  3La2O3,  SO3+zH2O.     (Cleve, 

B.  11.  910.) 

Lanthanum  sulphate,  La2(SO4)3. 

Anhydrous.  Much  less  sol.  in  warm  than 
in  cold  H2O.  1  pt.  is  sol.  in  less  than  6  pts. 
H2O,  if  added  in  small  portions  thereto  at 
2-3°,  and  the  temperature  not  allowed  to  rise 
to  13°;  but  if  heated  to  30°,  La2(SO4)3+9H2O 
separates  out  until  the  solution  is  solid. 
(Mosander.) 

100  pts.  H2O  dissolve  2.208  pts.  La2(SO4)« 
at  16.5°;  2.130  pts.  at  18°;  1.641  pts.  at  34°.  - 

See  also  under  +9H2O. 

The  solubility  of  La2(SO4)3  in  H2O  is  dim- 
inished by  the  presence  of  (NH4)2SO4,  K2S04 
or  Na2SO4.  (Barre,  C.  R.  1910,  151.  871.) 

Solubility  in  (NH4)2SO4+Aq  at  18°. 


Pts.  per  100  pts. 
H20 

Solid  phase 

§ 

m 

g 

6 
S 

3 

0.00 
4.011 

8.727 
18.241 
27.887 
36.112 
47.486 
53.823 
65.286 
73.782 

2.130 
0.393 
0.279 
0.253 
0.476 
0.277 
0.137 
0.067 
0.0117 
0.0033 

La2(SO4)3+9H20 

La2(S04)3,  (NH4)2S04+2H20 
u 

tt 
if 
tt 

2La2(S04)3,  5(NH4)2S04 
La2(S04)3,  5(NH4)2S04 

" 

(Barre.) 
Solubility  in  K2SO4+Aq  at  16.5°. 


Pts.  per  100  pts. 
H20 

Solid  phase 

La2(SO4)8+9H2O 
La2(S04)3,  K2S04+2H20 

u 

La2(SO4)3,  5K2SO4 
tt 

K2SO4 

La2(SO4)s 

0.00 

0.247 
0.496 
0.846 
1.029 
1.516 

2.198 
0.727 
0.269 
0.185 
0.054 
0.022 

(Barre.) 


SULPHATE,  LEAD 


979 


Solubility  in  Na2SO4+Aq  at  18°. 

La2(SO4)3,  4K2SO4.     As  above.     (Cleve.) 

Pts.  per  100  pts. 

2La2(S04)8,  9K2SO4.    As  above.     (Cleve.) 

H2O 

Solid  phase 

Lanthanum   rubidium   sulnha.tfc 

Na2SO4 

La2(S04)s 

JL/CJiitlltfUiUiiA      lU.UlvilU-l.li.      oU.ljJliC4.LCy 

La2(S04)3,  Rb2S04. 

0.00 

2.130 

La2(SO4)3+9H2O 

(Baskerville,  J.  Am.  Chem.  Soc.  1904,  26. 
67.) 

0.395 
0.689 
0.774 

0.997 
0.353 
0.299 

La2(SO4)3,  Na2SO4 
tt 

+2H2O.    (Baskerville.) 
3La2(SO4)3,  2Rb2SO4.     (Baskerville.) 

1.136 

0.  129 

(i 

2^480 

0^044 

« 

Lanthanum    sodium    sulphate,     La2(SO4)8, 

3.802 

0.019 

(( 

Na2SO4+2H20. 

5.548 

0.016 

ii 

SI.  sol.  in  H20.     (Cleve.)     (Barre,  C.  R. 

1910,  161.  872.) 

(Barre.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J 
1898,  20.  830.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.4329.) 

+9H2O.  Sol.  in  42.5  pts.  H2O,  calculated 
as  anhydrous  salt,  at  23°,  and  115  pts.  H20 
at  100°.  (Mosander.) 

Solubility  in  H2O. 
100  pts.  H2Q  dissolve  pts.  La2(SO4)3  at  t°. 


t 

Pts.  La2(SO4)3 

ar 

0 

3.02 

•p 

14 

2.60 

r 

30    ' 

1.90 

50 

1.49 

75 

0.94 

Li 

100 

0.68 

(Muthmann  and  Rolig,  B.  1898,  31.  1723.) 

, 

Solubility  in  H2SO4+Aq  at  25°. 

C 

In  100  g.  of  the 

86 

Normality 
H2SO4 

liquid  are  dissolved 

Solid  phase 

PI 

g.  oxide 

g.  sulphate 

i  ( 

at 

0 

1.43 

2.483 

La2(SO4)3+9H2O 

12 

0.505 

1.69 

2.934 

1.10 

1.796 

3.118 

so 
Z. 

2.16 

1.818 

3.156 

3.39 

1.42 

2,465 

4.321 

1.11 

1.927 

\^ 

6.685 

0.5309 

0.9217 

j*j 

9.68 

0.2659 

0.4617 

i  *«i 

12.60 

0.2136 

0.3709 

1  o 

15.15 

0.177 

0.3073 

It 

(Wirth,  Z.  anorg.  1912,  76.  189.) 

Lanthanum  hydrogen   sulphate,  La(SO4H)3. 
(Brauner,  Z.  anorg.  1904,  38.  330.) 

Lanthanum  potassium  sulphate,    La2(SO4)3, 
K2S04+2H20. 

La2(SO4)3,  5K2SO4.  (Barre,  C.  R.  1910, 
151.  872.) 

La2(SO4)3.  3K2SO4.  SI.  sol.  in  H2O.  Insol. 
in  sat.  K2SO4+Aq.  (Cleve.) 


Lead  sulphate,  basic,  2PbO,  SO3. 

Not  completely  insol.  in  H2O.  Decomp.  by 
acids,  even  dil.  HC2H3O2+Aq,  with  forma- 
tion of  PbSO4.  (Barfoed,  1869.) 

0.050  millimole  calc.  as  Pb  is  sol.  in  1  1. 
H2O  at  18°.  (Pleissner,  C.  C.  1907,  II. 
1056.) 

5PbO,  3SO3.  (Frankland,  Proc.  Roy.  Soc. 
46.  364.) 

Pb3O4,  2SO3.    (Frankland.) 

3PbO,PbSO4+H2O.  Ppt.  (Stromholm,  Z. 
anorg.  1904,  38,  442.) 

Pb4(SO4)(OH)2.  0.106  millimole  calc.  as 
Pb  is  sol.  in  1  liter  H2O  at  18°.  (Pleissner, 
C.  C.  1907.  II,  1056.) 

Lead  sulphate,  PbS04. 

Sol.  in  22,816  pts.  H2O  at  11°.  (Fresenius, 
A.  69.  125.) 

Sol.  in  31,569  pts.  H2O  at  15°.  (Rodwell, 
C.  N.  11.  50.) 

Sol.  in  13,000  pts.  H2O.  (Kremers;,  Pogg. 
86.  247.) 

Calculated  from  electrical  conductivity  of 
PbSO4+Aq,  1 1.  H2O  dissolves  46  mg.  PbSO4 
at  18°.  (Kohlrausch  and  Rose,  Z.  phys.  Ch. 
12.  241.) 

4.23  XHHgr.  are  dissolved  in  1  liter  of  sat. 
solution  at  20°;  4.41  X 10  2  at  25°.  (Bottger, 
.  phys.  Ch.  1903,  46.  604.) 

1  1.  H2O  dissolves  41  mg.  PbSO4  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1904,  60. 

16.) 

o!l26  millimole  Pb  is  sol.  in  1  liter  H2O  at 
;°.    (Pleissner.  C.  C.  1907,  II.  1056.) 
40  mo-  are  dissolved  in  1  1.  of  sat.  solution 
18°.     (Kohlrausch,    Z.  phys.  Ch.  1908,  64. 
'8.) 

0.0824  g.  PbSO4  is  sol.  in  1000  cc.  H2O 
at  18°  and  also  at  100°.  The  fact  that  PbSO4 
dissolves  in  H2O  is  ascribed  to  hydrolysis,  and 
n  support  of  this  it  is  shown  that  the  solubil- 
ty  of  hydrated  oxide  of  lead,  PbO,  H2O,  in 
dil.  H2SO4  is  the  same  as  the  solubility  of 
>bSO4  in  H2O.  (Sehnal,  C.  R.  1909,  148. 
395  ) 

1  1.  H2O  dissolves  26  mg.  at  18°;  30  mg. 
it  25°;  38  mg.  at  37°.  (Beck  and  Stegmiiller, 
Arb.  K.  Gesund.  Amt.  1910,  34.  447.) 


980 


SULPHATE,  LEAD 


Solubility  in  H2O  at  tc 
(Millimols  per  1.) 


t° 

PbSO4 

18 
25 
37 

0.126 
0.144 
0.183 

(Beck 


and    Stegmuller,    Arb.    K.    Gesund. 
Amt.  1910,  34.  446.) 

Sol.  in  hot  cone.  HCl+Aq.     (Fresenius.) 
Solubility  of  PbSO4  in  HCl+Aq. 


Sp.  gr.  of 
HCl+Aq 

%  HCl  in 
HCl+Aq 

Pts.  HCl+Aq 
for  1  pt.  PbSO4 

1.0519 
1.0800 
1.1070 
1.1359 
1  .  1570 

10.602 
16.310 
22.010 
27.525 
31.602 

681.89 

281  .  73 
105.65 
47.30 
35.03 

(Rodwell,  Chem.  Soc.  16.  59.) 

Solubility  of  PbSO4  in  HCl+Aq  at  t°. 
(Millimols.  per  1.) 


t° 

0.1N 

0.2N 

0.3N 

0.4N 

18 

0.126 

1.72 

2.67 

3.63 

25 

0.144 

2.07 

3.14 

4.29 

37 

0.183 

2.63 

4.06 

5.43 

(Beck  and  Stegmuller,  Arb.  K.  Gesund.  Amt. 
1910,  34.  446.) 

Above  measurements  in  HCl+Aq  show 
solubility  directly  proportional  to  the  hydro- 
gen ions.  (Beck  and  Stegmuller.) 

Sol.  in  HNO3+Aq,  and  more  sol.  in  hot  or 
cone,  than  in  cold  or  dil.  HNO3+Aq. 

Sol.  in  172  pts.  HNO3+Aq  of  1.144  sp.  gr. 
at  12.5°.  (Bischof.) 

Pptd.  from  HNO3  solution  by  dil.  H2SO4  + 
Aq  and  not  by  H2O.  (Bischof,  1827.) 

Solubility  of  PbSO4  in  HNO3+Aq. 


Sp.  gr.  of 
HNOa+Aq 


1.079 
1.123 
1.250 
1.420 


%  HNOs  in 
HNOs+Aq 


11.55 
17.50 
34.00 
60.00 


Pts.  HNOs+Aq 
for  1  pt.  PbSO4 


303.10 
173.75 

127.48 
10282.78 


(Rodwell,  Chem.  Soc.  16.  59.) 

Solubility  in  HNO3  at  18°. 
(Millimols  per  1.) 


HNOs 


0.1N 
0.2N 
0.3N 
0.4N 


PbS04 


0.506 
0.844 
1.13 

1.44 


(Beck  and  Stegmuller.) 


Sol.  in  36,504  pts.  dil.  H2SO4+Aq.  (Fre- 
senius.) See  also  under  solubility  in  alcohol. 

SI.  sol.  in  cone.  H2SO4,  from  which  it  is 
partially  pptd.  by  H2O  or  completely  by 
alcohol.  (Fresenius.) 

100  pts.  cone.  H2SO4  dissolve  6  pts.  PbSO4. 
(Schultz,  Pogg.  133.  137.) 

Cone.  H2SO4  dissolves  0.005  pt.  PbSO4. 
(Ure.) 

100  pts.  H2SO4  dissolve  0.13  pt.  PbSO4,  and 
100  pts.  fuming  H2SO4  dissolve  4.19  pts. 
(Struve,  Z.  anal.  9.  31.) 

More  sol.  in  commercial  H2SO4  than  in  the 
more  cone.  acid.  (Hayes.) 

100  pts.  H2SO4+Aq  of  1.841  sp.  gr.  dissolve 
0.039  pts.  PbSO4;  of  1.793  sp.  gr.  dissolve 
0.011  pt.  PbSO4;  of  1.540  sp.  gr.  dissolve 
0.003  pt.  PbSO4. 

Presence  of  SO2  does  not  increase  the  solu- 
bility; HNO3  increases  the  solubility  some- 
what, i.  e.,  100  pts.  H2SO4+Aq  of  1.841  sp. 
gr.  with  5  pts.  HNO3  of  1.352  sp.  gr.  dissolve 
0.044  pt.  PbSO4;  100  pts.  H2SO4  of  1.749  sp. 
gr.  with  5  pts.  HNO3  of  1.352  sp.  gr.  dissolve 
0.014  pt.  PbSO4;  100  pts.  H2SO4  of  1.512  sp. 
gr.  with  5  pts.  HNO3  of  1.352  sp.  gr.  dissolve 
only  a  trace. 

Nitrous  oxides  do  not  increase  the  action. 
(Kolb,  Dingl.  209.  268.) 

Solubility  in  dil.  H2SO4+Aq  at  18°. 
(G.  per  1.) 


0 

0.0049 

0.0098 


PbS04 


0.0382 
0.0333 
0.0306 


H2S04 


0.0245 
0.0490 
0.4904 


PbS04 


0.0194 
0.0130 
0.0052 


(Pleissner,  Arb.  K.  Gesund.  Amt.  1907,  26. 
384.) 

A  trace  of  H2SO4  has  a  considerable  effect 
in  reducing  the  solubility  of  PbSO4  in  H20. 
(Sehnal,  C.  R.  1909,  148.  1395.) 

Solubility  in  dil.  H2SO4+Aq  at  20°. 
(G.  per  1.) 


H2SO4 


0 

0.0098 

0.0196 


PbS04 


0.082 
0.051 
0.025 


H2SO4 


0.0980 
0.4900 
0.9800 


PbS04 

0.013 
0.006 
0 


(Sehnal.) 

Pptd.  from  solution  in  H2SO4  by  HCl. 
(Bolley,  A.  91.  113.) 

Not  more  insol.  in  dil.  HC2H3O2+Aq  than 
in  H2O.  (Bischof.) 

Solubility  in  other  acids  is  prevented  by 
great  excess  of  H2SO4.  (Wackenroder.) 

Sol.  in  warm  NH4OH+Aq,  separating  on 
cooling.  Completely  sol.  in  warm  K.OH  or 
NaOH+Aq. 


SULPHATE,  LEAD 


981 


Decomp.  by  boiling  with  K2CO3,  Na2CO3, 
and  (NH4)2CO3+Aq. 

Sol.  in  NH4  salts  +Aq,  but  repptd.  by 
H2SO4+Aq.  (Fresenius,  A.  69.  125.) 

The  best  solvents  of  the  NH4  salts  are  the 
nitrate,  citrate,  and  tartrate;  the  two  latter 
should  be  strongly  alkaline  with  NH4OH+Aq. 
( Wackenroder . ) 

Sol.  in  NH4Cl+Aq  at  12.5-25°. 

SI.  decomp.  by  NaCl+Aq.    (Bley.) 

1  1.  sat.  NaCl  +Aq  dissolves  0.66  g.  PbSO4. 
(Becquerel.) 

Sol.  in  100  pts.  cold  cone.  NaCl+Aq,  and 
PbCl2  is  deposited  after  a  few  hours.  (Field.) 


Solubility  in  ammonium  acetate  +Aq  at  25°. 

NH4C2H302 
Millimol.  per.  1. 

Solubility  of  PbSO4 

Millimols.  per  1. 

g.  per  1. 

0.0 
103.5 
207.1 
414.1 

0.134 
2.10 
4.55 
10.10 

0.041 
0.636 
1.38 
3.06 

Solubility   of  PbSO4  in   NaCl+Aq  at   18°. 
(Millimols  per  1.) 

oouu  pnase,  jruov^f  .ru-LY2^ow4j2. 

Composition  of  the  solutions 

NaCl 

PbS04 

°7 
KC2H3O2 

% 

Pb(C2H302)2 

% 
KC2H302 

Pb(C2H3O2)2 

0.1N 
0.2N 
0.3N 
0.4N 

0.546 
0.904 
1.28 
1.68 

4.33 
9.03 
17.81 
22.07 

2.54 
3.55 
5.43 
5.95 

26.58 
28.82 
28.93 

9.83 
11.40 
19.41 

(Beck  and  Stegmiiller,  Arb.  K.  Gesund.  Amt. 
1910,  34.  446.) 

(Fox,  Chem.  Soc.  1909,  95.  887.) 

Sol.  in  Fe2Cl6-t-Aq.      (Fresenius,  Z.  anal 
19.  419.) 

Sol.  in  Na2S2O3+Aq.     (Lowe.) 
Sol.  in  (NH4)2SO4+Aq.    (Rose.) 

Solubility  of  PbSO4+PbSO4,  K2SO4  in  H2O 


0 

22 


g.  in  100 

cc.  of 
solution 


0.195 
0.396 


Mol.  in 
100  cc.  of 

solution 


0.0112 
0.0227 


Solid  phase 


K2SO4,  PbSO4+PbSO4 


(Bronsted,  Z.  phys.  Ch.  1911,  77.  316.) 
Sol  in  47  pts.  NH4C2H3O2+Aq)  1.036  sp, 
gr.),  and 969  pts.  NH4NO3+Aq  (1.269  sp.  gr.): 
from  the  solution  in  NH4C2H3O2  it  is  pptd.  by 
H2SO4  or  K2SO4;  from  solution  in  NH4NO3 
by  K2SO4,  but  not  by  H2SO4.  (Bischof.) 

Sol.  in  acetates  of  NH4,  Na,  K,  Ca,  Al,  and 
Mg.    (Mercer.) 

Solubility  in  NH4C2H3O2+Aq.  Excess  o 
PbSO4  was  boiled  with  solution  o 
NH4C2H3O2+Aq  of  varying  cone. 


G. 

NH4.C2H302 
in  100  cc. 

g.  PbSO4  contained  in  5  cc.solution 

Hot 

Cooled 

Cooled  24  hrs. 

28 

30 

32 
35 
37 
40 
45 

0.356 
0.418 
0.494 
0.513 
0.529 
0.539 
0.555 

0.451 
0.452 

0.488 

0'.224 
0.242 

0.238 
0.263 

(Dunnington  and  Long,  Am.  Ch.  J.  1899,  22. 

218.) 

Noyes  and  Whitcomb,  J.  Am.  Chem.  Soc. 
1905,  27.  756.) 

Solubility  in  KC2H3O2+Aq  at  25°. 


100  pts.  H20  containing  a  drop  of  HC2H3O2 
and  2.05  pts.  NaC2H3O2  dissolve  0.054  pt. 
PbSO4;  containing  8.2  pts.  NaC2H3O2  dis- 
solve 0.900  pt.  PbSO4;  containing  41.0  pts. 
NaC2H3O2  dissolve  11.200  pts.  PbSO4. 
Dibbits,  Z.  anal.  1874,  13.  139.) 

Solubility  in  NaC2H3O2+Aq  at  25°. 


Composition  of  the  solutions 


%  Na  acetate  %  PD  acetate    % 


6.69 
11.76 
16.90 
19.92 
21.51 

6.95 


0.78 
2.73 
5.70 
8.24 
10.75 
0.81 


0.34 
1.26 
2.49 
3.60 
4.68 
0.35 


%H20 


92.19 
84.25 
74.91 
68.24 
63.10 
91.90 


The  proportion  of  sulphate  in  solution  in 
each  case  corresponded  with  the  amount  of 
Pb  present,  but  was  calculated  to  sodium 
sulphate,  since  Na2SO4+10H2O  cryst.  from 
the  solutions  on  cooling.  The  solid  phase  in 
these  solutions  was  PbSO4. 

(Fox,  Chem.  Soc.  1909,  96.  887.) 

Sol.  in  Mn(C2H3O2)2,  Zn(C2H3O2)2, 
Ni(C2H3O2)2,  and  Cu(C2H3O2)2,  but  not  in 
Hg(C2H3O2)2  or  AgC2H3O2+Aq. 

Solubility  in  KC2H3O2+Aq  is  not  less  than 
that  in  NaC2H3Oa+Aq.  (Dibbits,  Z.  anal. 
13.  137.) 

Insol.  in  Pb(C2H3O2)2-hAq.    (Smith.) 

Sol.  in  basic  lead  acetate  +Aq,  but  not  in 
neutral  Pb(C2H3O2)2+Aq.  (Stammer,  Z. 
anal.  23.  67.) 

12.2  pts.  Ca(C2H3O2)2  in  very  dil.  solution 
dissolve  1  pt.  PbSO4.  (Stadel,  Z.  anal.  2. 180.) 

Sol.  in  Al(C2H3O2)3+Aq.    (Lennsen.) 


982 


SULPHATE,  LEAD  HYDROGEN 


Very  easily  and  abundantly  sol.  in  NH 
tartrate  +Aq.  (Wohler,  A.  34.  235.) 

Even  when  native,  easily  sol.  in  NH4  citrate 
+Aq.  (Smith.) 

Insol.  in  alcohol  (18%)  and  H2SO4  when 
NH4  acetate,  K  tartrate,  or  NH4  succinate  are 
present.  Insol.  in  alcohol  (18%)  and  H2SO 
or  (NH4)2SO4  when  Na  acetate,  Na  or  NH4 
oxalate  are  present.  Sol.  in  NH4  cfo'citrate  anc 
K  Zricitrate  in  presence  of  H2SO4;  in  NH4 
succinate  and  NH4  acetate  in  presence  oi 
(NH4)2SO4;  and  in  NH4  citrate  in  presence  of 
H2SO4  or  (NH4)2SO4.  (Storer,  C.  N.  21.  17. 

Alcohol  (59%)  alone,  or  with  ethylsul- 
phuric  acid  or  sugar,  does  not  dissolve  Pb  by 
3  months  action.  (Storer.) 

Insol.  in  acetone.  (Naumann,  B.  1904 
37.  4329);  methyl  acetate.  (Naumann 
B.  1909,  42.  3790);  ethyl  acetate.  (Naumann 

B.  1910,  43.  314.) 

Min.  Anglesite.  Sol.  in  cold  citric  acid  +Aq 
(Bolton,  C.  N.  37.  14.) 

Lead  hydrogen  sulphate, PbSO4,  H2S04+H2O, 
Decomp.  by  H2O. 

Lead  p^/rosulphate,  Pb  S2O7. 
Decomp.  by  H2O.(Schultz.) 

Lead  potassium  sulphate,  PbSO4,  K2SO4. 

When  PbSO4  is  added  to  potassium  acetate 
+Aq  at  25°  a  double  salt,,  PbK2(SO4)2  is 
formed.  This  salt  is  insol.  in  the  solution 
which  contains  only  potassium  acetate  and 
lead  acetate.  (Fox,  Chem.  Soc.  1909,  96. 
882.) 

Decomp.  by  H2O.  Stable  only  in  solutions 
of  K2S04,  containing  at  least  0.56%  K2SO4 
at  7°;  0.62%  at  17°;  1.09%  at  50°;  1.37%  at 
75°:  1.69%  at  100°.  (Barre,  C.  R.  1909,  149. 
294.) 

Lead   sulphate   chloride,    PbSO4,   2PbCl2+ 
H2O. 

Insol.  in  H2O  or  NaCl+Aq.     (Becquerel, 

C.  R.  20.  1523.) 

Lead  sulphate  fluoride,  PbSO4,  2PbF2. 


Sat.  Li2SO4+Aq  contains  at: 

—20°     —16°     —15°     —12° 

18.4       22.5       22.6       24.4  %  Li2SO4. 

-4°          +15°         +90° 
25.7        25.3          23.9  %  Li2SO4. 
(Etard,  A.  ch.  1894,  (7)  2.  547.) 


Sat.  solution  boils  at  105°.    (Kremers.) 
Sp.  gr.  of  Li2SO4+Aq  at  19.5°  containing: 

6.5       7.4       12.5        15.3%Li2SO4, 

1.05      1.06      1.098      1.118 


22.6          24.4 
1.167        1.178 

(Kremers,  Pogg.  114.  47.) 


29.4  %Li2SO4. 
1.208 


Sp.  gr.  of  Li2SO4+Aq  at  15°  containing  5% 
Li  2SO4  =  1.0430;     10%     Li2SO4  =  1.0877. 
(Kohlrausch,  W.  Ann.  1879 


1.) 


Sp.  gr.  of  Li2S04+Aq  at  25°. 


Concentration  of  Li2SC>4 
+Aq 

Sp.  gr. 

1  —  normal 

V«—     " 

V4—         " 

Vr-     " 

1.0453 
1.0234 
1.0115 
1.0057 

(Wagner,  Z.  phys.  Ch.  1890,  6.  38.) 


Sp.  gr.  of  Li2SO4+Aq. 


^Li2S04  g.  in  1000  g.l 
of  solution           (2J 

Sp.  gr.  16°/16° 

0 
2.9198 
16.0461 

1.000000 
1.002589 
1.014093 

(Dijken,  Z.  phys.  Ch.  1897,  24.  109.) 


Sp.  gr.  of  Li2SO4+Aq  at  20°. 


434.) 

Lithium  sulphate,  Li2SO4. 
More  sol.  in  cold  than  in  hot  H2O. 

100  pts.  H2O  dissolve  34.6  pts.  Li2SO4  at  18°.     (Witt- 
stein.) 

100  pts.  H2O  dissolve  pts.  Li2SO4  at  t° 

Normality  of 
Li2S04+Aq 

%  Li2S04 

Sp.  gr. 

2.60 
1.96 
1.708 
1.320 
0.747 

23.48 
18.53 
16.41 
13.01 
7.71 

1.2330 
1  .  1650 
1  .  1449 
1.1133 
1.0678 

(Forchheimer,   Z.   phys.   Ch.    1900,   34.  24.) 

Insol.  in  SO3.    (Weber,  B.  17.  2497.) 
10  ccm.  of  sat.  Li2SO4  in  absolute  H2S04 
contain  approx.  2.719    g.  Li2SO4.     (Bergius, 
Z.  phys.  Ch.  1910,  72.  355.) 

t° 

Pts. 
Li2SO4 

t° 

Pts. 
Li2S04 

t° 

Pts. 

Li2SO4 

0 

20 

35.34 
34.36 

45 
65 

32.38 
30.3 

100 

29.24 

(Kremers, 

Pogg.  95. 

468.) 

SULPHATE,  LITHIUM  THALLIC 


Solubility  in  H2SO4+Aq  at  30°. 

Solubility 

of  Li2SO4  in  alcohol  +Aq  at  30°. 

Composition  of  the  solution 

Solid  phase  Li2SU4,  H2U. 

%Hb2Sof' 

\SSo7" 

Solid  phase 

G.  per  100  g. 

sat.  solution 

C2H5OH 

T  '  SO 

12         4 

P  H  OH 

T  '  SO 

12         4 

5 

.05 

22 

.74 

Li2SO4,  H2O 

2      5 

12 

.23 

20 

.45 

0 

25.1 

47.28 

3.04 

15 

.37 

19 

.11 

11.75 

16.16 

58.59 

1.22 

16 

.60 

19 

.10 

21.19 

11.52 

69.39 

0.4 

32 

.70 

13 

.37 

29.40 

8.17 

80.74 

0 

36 

A  O 

.90 

11 

i  r\ 

.90 

ri-r 

33.31 

6.66 

94.11 

0 

42 

48 

.98 
.00 

10 

10 

.57 
.20 

(Schreinemakers    and 

van    Dorp,     Chem. 

52 

.72 

11 

.44 

Weekbl.  1906.  3.  557.) 

54 

.54 

12 

.92 

55 

.08 

13 

.69 

Li2SO4 

56 

.30 

13 

.87 

Insol.  in  methyl  acetate   (Naumann,   B. 

61 

.46 

17 

.10 

1909,   42. 

3790);  ethyl  acetate   (Naumann. 

61 

.82 

17 

.00 

B.  1904,  37 

.  3601)  ;  acetone.    (Eidmann,  C.  C, 

62 
62 

.14 
.49 

17 
18 

.97 
.89 

Li2SO4  H2SO4 

1899,  II.  1014;  Naumann,  B.  1904, 
+H2O.    Very  si.  efflorescent. 

37.  4329.) 
(Rammels- 

65 

.70 

16 

.55 

berg.) 

69 

.40 

13 

.75 

Aq.  solution  contains  25.1%  Li2SO4  at  30°. 

77 

.30 

11 

.31 

(Schreinemakers,  C.  C.  1910,  I.  1801);  24.3 

78 

.23 

11 

.64 

g.  at  50°. 

(Schreinemakers  and  Cocheret. 

81 

.20 

13 

.28 

Chem.  Weekbl.  1905,  2.  771.) 

81 

.70 

13 

.85 

82 

.30 

15 

.50 

83 

.43    . 

15 

.65 

Lithium  hydrogen  sulphate,  LiHS04. 

(Van  Dorp,  Z.  phys.  Ch.  1910,  73.  289.) 


Solution  in  H2SO4  contains  17.2%  Li2SO4 
at  30°.  (Van  Dorp,  Z.  phys.  Ch.  1913,  86. 
112.) 


Solubility  of  Li2SO4+Th(SO4)2  in  H2O 
at'  25°. 

Solid  phase,  Th(SO4)2. 
G.  in  100  g.  H2O. 


Li2S04 

Th(S04)2 

Li2S04 

Th(S04)2 

0.0 
2.57 
4.93 
6.98 
9.23 

1.722 
4.13 
6.20 
7.95 
9.68 

11.13 
13.18 
16.12 
20.49 
16.92 

11.05 
12.54 
14.52 
16.92 

18.87 

(Barre,  Bull.  Soc.  1912,  (4)  11.  647.) 


Easily  sol.  (Kastner),  si.  sol.  (Berzelius)  in 
alcohol. 


Cryst.  from  H2SO4.    (Gmelin.) 

LiH3(SO4)2.  Cryst.  from  H2SO4.  (Schultz, 
Pogg.  133.  137.) 

Li2SO4,  7H2SO4.  (Bergius,  Z.  phys.  Ch. 
1910,  72.  355.) 


Lithium  potassium   sulphate,   Li2SO4,K2SO4. 

This  is  the  only  compd.  of  Li2SO4  and 
K2SO4  which  exists  below  100°.  (Spielrein, 
C.  R.  1913,  157.  48.) 

K4Li2(SO4)3.  (Knobloch.)  Has  the  for- 
mula K2Li8(SO4)5+8H2O,  according  to  Ram- 
melsberg. 

Lithium  sodium  sulphate,  Na3Li(SO4)2  + 
6H2O. 

Na4Li2(SO4)3+9H2O. 

Na2Li8  (SO4)  5  +5H2O  .    (Rammelsberg.  ) 

Do  not  exist.     (Troost.) 

Li2SO4,  Na2SO4+5.5H2O.  Exists  from 
0°-16°. 

+3H2O.   Exists  from  32°-100°. 

Li2SO4,  3Na2SO4+12H2O.  Exists  from 
16°-24°. 

4Li2SO4,  Na2SO4+5H2O.  Exists  from 
24°-32°. 

(Spielrein,  C.  R.  1913,  167.  47.) 


Lithium  thallic  sulphate,  LiTl(SO4)2+3H2O. 
(Meyer  and  Goldschmidt,  C.  C.  1903,  I. 

495.) 


984 


SULPHATE,  LITHIUM  TITANIUM 


Lithium  titanium  sulphate, 

Li2TiO2(SO4)2+7H2O. 
Less     hygroscopic     than     K     compound. 
(Mazzuchelli  and  Pontanelli,  C.  C.  1909,  II. 
420. 


Lithium  uranyl  sulphate,  Li2SO4,  UO2SO4+ 

4H2O. 
(de  Coninck,  Chem.  Soc.  1905,  88.  (2)  530. 


Magnesium  sulphate  basic, 

6Mg(OH)2,  MgSO4+3H2O. 
SI.  sol.  in  cold  or  hot  H2O. 
Sol.    in   HCl+Aq.      (Thugutt,    Z.    anorg. 
1892,  2.  150.) 


Magnesium  sulphate,  MgSO4. 

Anhydrous.  Very  slowly  sol.  in  H2O;  sol. 
in  hot  cone.  H2SO4,  less  in  HC1,  and  HNO3  + 
Aq. 

+H2O.  Min.  Kieserite.  Easily  sol.  in 
warm,  but  slowly  dissolved  by  cold  H2O. 

100  g.  sat.  solution  at  83°  contain  40.2  g. 
MgSO4.  (Geiger,  Dissert.  1904.) 

+6H2O,  and  +7H2O.  The  latter  exists  in 
two  modifications;  (a)  hexagonal,  and  (6)  the 
ordinary  or  rhombic  salt. 

MgSO4+Aq,  which  on  cooling  or  keeping 
in  closed  vessels  has  deposited  MgSO4+6H2O, 
always  contains  for  100  pts.  H2O  at: 

0°          10°        20° 
40.75    42.23    43.87  pts.  MgS04. 


If  only  hexagonal  MgSO4+7H20  has  been 
deposited,  then  the  mother  liquor  contains 
for  100  pts.  H2O  at: 

0°          10°         20° 
34 . 67    38 . 71    42 . 84  pts.  MgSO4. 

Solutions  prepared  from  rhombic  MgSO4+ 
7H2O  contain  for  100  pts.  H2O  at: 

0°          10°         20° 
26.0      30.9      35. 6  pts.  MgSO4. 
(Lowel.) 

These  results  may  be  given  in  tabular  form 
as  follows: 


Temp. 

A  sat.  aqueous  solution  of 
MgSO4+7H2O  (a)  contains 
for  100  pts.  H2O 

Anhydrous 
MgSO4 

7H2O  (a) 
sale 

0° 

34.67 

111.74 

10° 

38.71 

133.67 

20° 

42.84 

159.61 

Temp. 

A  sat  aqueous  solution  of  MgSC>4  +6H2O 
contains  for  100  pts.  HzO 

Anhydrous 
MgSCU 

6H20 
salt 

7H20 
salt 

0° 

40.75 

122.22 

146.02 

10° 

42.32 

129.44 

155.53 

20° 

43.87 

137  .  72 

167.97 

It  is  seen  from  table  that  at  the  same  temp, 
the  6H2O  salt  is  more  sol.  than  the  7H2O  (6) 
salt,  and  the  latter  is  more  sol.  than  7H2O  (a) 
salt;  that  the  solubility  of  the  7H2O  (6)  salt 
increases  rapidly  from  0°  to.  20°;  that  the 
6H2O  salt  is  not  much  more  sol.  at  20°  than  at 
0°,  and  at  20°  the  7H2O  (6)  salt  is  nearly  as 
sol.  as  the  6H2O  salt.  (Lowel,  A.  ch.  (3)  43. 
405.) 

100  pts.  H2O  at  t°  dissolve  pts.  MgSO4.  G  L  =  accord- 
ing to  Gay-Lussac  (A.  ch.  (2)  11.  311);  T  =accord- 
ing  to  Tobler  (A.  95.  198). 


t° 

G  L 

T 

t° 

G  L 

T 

0 
10 
20 
25 
30 
40 

25.8 
30.5 
35.0 

39!  8 
45.2 

24.7 
37.1 

50 
55 
60 
70 
80 
90 

49.7 

55.9 
60.4 
65.1 
70.3 

52^8 

100  pts.  H2O  at  105.5°  dissolve  135.2  pts.  MgSO4. 
(Griffiths.) 

MgSO4+Aq  sat.  at  17.5  has  sp.  gr.  =1.2932,  and 
contains  55.57  %  MgSO4+7H2O,  or  100  pts.  H2O 
dissolve  125.06  pts.  MgSO4+7H2O,  or  60  pts.  MgSO4, 
at  17.5°.  (Karsten.) 

100  pts.  H2O  at  0°  dissolve  53.8  pts.,  and  125  pts. 
at  ord.  temp.  (Otto-Graham.) 

Sol.  in  2  pts,  cold,  and  0.5  pt.  boiling  H2O.  (Four- 
croy.) 

The  aqueous  solution  contains  for  100  pts.  H2O 
92.217  pts.  MgSO4  +7H2O  at  15°.  (Michel  and  Krafft.) 

I  pt.  MgS04+7H«0  is  sol.  in  0.933  pt.  H2O  at  15° 
(Gerlach);  in  0.92  pt.  H2O  at  23°  (Schiff). 

100  pts.  H20  dissolve  28.067  pts.  MgSO4  at  0°. 
(Pfaff,  A.  99.  224.) 

100  pts.  H2O  dissolve  pts.  MgSO4  at  t°. 


Temp. 

A  sat.  aqueous  solution  of 
MgSO4+7H2O  (6)  contains 
for  100  pts.  H2O 

t 

Pts.  MgS04 

0 
17.9 
24.1 

26.37 
33.28 
35.98 

Anhydrous 
MgS04 

7H2O  (6) 
salt 

0° 

26.0 

73.31 

(Diacon,  J.  B.  1886.  62.) 

100  pts.  MgSO4+Aq  sat.  at  18-20°  contain 
25.67-26.38  pts.  MgSO4.     (v.  Hauer,  J.  pr. 
98.  137.) 

10° 

30.9 

93.75 

20° 

35.6 

116.54 

SULPHATE,  MAGNESIUM 


985 


Solubility  in  100  pts.  H2O  at  t°,  using 
MgSO4+7H2O. 

M.-pt.  of  MgSO4+7H2O  is  70°.     (Tilden, 
Chem.  Soc.  46.  409.) 

Pts. 

Pts. 

Pts. 

t° 

MgSC>4 

t° 

MgSO* 

t° 

MgSO4 

MgSO4+Aq    with    sp.    gr.    1.50    contains    44.4    % 

MsSO4;  sp.  gr.  1.42,  39%;  sp.  gr.  1.30,  30%  MgSOi. 

0 

26.9 

37 

44.2 

74 

61.4 

(Dalton.) 

1 

27.4 

38 

44.7 

75 

61.9 

2 
3 

27.9 
28.3 

39 
40 

45.2 
45.6 

76 

77 

62.3 
62.8 

Sp.  gr.  of  MgSO4+Aq  sat.  at  15°  =  1.275 
(Michel  and  Krafft);  at  8°  =  1.267  (Anthon); 

4 

28.8 

41 

46.1 

78 

63.2 

at  18.75°  =  1.293  (Karsten.). 

5 

29.3 

42 

46.5 

79 

63.7 

6 

29.7 

43 

47.0 

80 

64.2 

7 

30.2 

44 

47.5 

81 

64.6 

Sp.  gr.  of  MgSO4+Aq  at  15°. 

8 

30.6 

45 

48.0 

82 

65.1 

9 

31.1 

46 

48.4 

83 

65.6 

%  MgS04 

Sp.  gr. 

%  MgSO4 

Sp.  gr. 

in 

01       K 

47 

4.0     Q 

04. 

fifi  0 

j.\J 

11 

Ol  .  O 

32.0 

T:  * 

48 

^±O  .  i) 

49.3 

OT: 

85 

oo  .  u 
66.5 

5 

1.054 

30 

1.326 

12 

32.4 

49 

49.8 

86 

67.0 

10 

1.108 

35 

1.384 

13 

32.9 

50 

50.3 

87 

67.5 

15 

1.161 

40 

1.446 

14 

33.4 

51 

50.7 

88 

68.0 

20 

1.215 

45 

1.511 

15 

33.8 

52 

51.2 

89 

68.4 

25 

1.269 

50 

1.580 

16 

°.4-   °. 

CO 

ci    7 

on 

AQ  q 

-LU 

17 
18 

OT:  .  O 

34.7 
35.2 

oo 
54 
55 

O-L  .  t 

52.2 
52.7 

<J\J 

91 
92 

UO  .  t/ 

69.4 
69.9 

(Calculated    from    Anthon    by    Schiff,    A. 
107.  303.) 

19 

35.7 

56 

53.2 

93 

70.4 

20 

36.2 

57 

53.6 

94 

70.9 

21 

36.7 

58 

54.1 

95 

71.4 

Sp.  gr.  of  MgSO4+Aq  at  23°. 

22 

37.1 

59 

54.5 

96 

71.9 

23 
24 

37.6 
38.0 

60 
61 

55.0 
55.5 

97 

98 

72.4 

72.8 

%  MgS04 
+7H20 

Sp.  gr. 

%  MgS04 
+7H2O 

Sp.  gr. 

25 

38.5 

62 

55.9 

99 

73.3 

26 

39.0 

63 

56.4 

100 

73.8 

1 

1.0048 

28 

1  .  1426 

27 

39.5 

64 

56.8 

101 

74.3 

2 

1.0096 

29 

1.1481 

28 

39.9 

65 

57.3 

102 

74.8 

3 

1.0144 

30 

.1536 

29 

40.4 

66 

57.7 

103 

75.2 

4 

1.0193 

31 

.1592 

30 

40.9 

67 

58.2 

104 

75.7 

5 

1.0242 

32 

.1648 

31 

41.4 

68 

58.6 

105 

76.2 

6 

1.0290 

33 

.1704 

32 

41.8 

69 

59.1 

106 

76.7 

7 

.0339 

34 

.1760 

33 

42.3 

70 

59.6 

107 

77.2 

8 

.0387 

35 

.1817 

34 

42.8 

71 

60.0 

108 

77.7 

9 

.0437 

36 

.1875 

35 

43.3 

72 

60.5 

108.4 

77.9 

10 

.0487 

37 

.1933 

36 

43.7 

73 

61.0 

11 

.0537 

38 

.1991 

12 

.0587 

39 

1  2049 

(Mulder,  calculated  from  his  own  and  other 
observations,  Scheik.  Verhandel.  1864.  52). 

13 

14 
15 

]0637 
.0688 
1.0739 

40 
41 
42 

1^2108 
1.2168 
1.2228 

100  pts.  H2O  dissolve  72.4  pts.  MgSO4  + 
7H2O  at  0°,  178  pts.  at  40°;  and  212.6  pts.  at 
49°.    (Tilden,  Chem.  Soc.  46.  409.) 
Supersat.  MgSO4+Aq  is  brought  to  crystal- 
lisation by  addition  of  crystal  of  MgSO4  + 
7H2O,     or    an    isomorphous    substance    as 
ZnSO4+7H2O,  NiSO4+7H2O,  FeSO4+7H2O, 
or  CoSO4+7H2O.      (Thomson,   Chem.   Soc. 

16 
17 
18 
19 
20 
21 
22 
23 
24 

1.0790 
1.0842 
.0894 
.0945 
.0997 
.1050 
.1103 
.1156 
.2109 

43 
44 
45 
46 
47 
48 
49 
50 
51 

1.2288 
.2349 
.2410 
.2472 
.2534 
.2596 
.2659 
.2722 
.2786 

35.  199.) 

25 

.1261 

52 

.2850 

Sat.  MgS04+Aq  contains  at: 

26 

27 

.1316 
.1371 

53 
54 

.2915 
.2980 

2°         7°         23°       67°        81° 

20.9     22.5     26.0     35.6     38.6%  MgSO4, 

(Schiff,  A.  113.  185.) 

94°       130°      145°      164°      188° 
41.5     45.3      38.0     29.3     20.4%  MgSO4. 
Readily  forms  supersat.  solutions. 
(Etard,  A.  ch.  1894,  (7)  2.  551.) 


SULPHATE,  MAGNESIUM 


Sp.  gr.  of  MgSO4+Aq  at  12°. 

Sp.  gr.  of  MgSO4+Aq  at  15°. 

%  MgS04 
+7H20 

Sp.  gr. 

%  MgSO4 
+7H20 

Sp.  gr. 

%  MgSCh          Sp.  gr. 

%  MgSO4 

Sp.  gr. 

5            1.0510 
10            1.1052 
15            1  .  1602 

20 
25 

1.2200 
1.2861 

1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 

1.0046 
.0096 
.0146 
.0196 
.0246 
.0296 
1.0346 
1.0396 
1.0446 
1.0497 
1.0548 
1.0599 
.0650 
.0702 
.0754 
.0807 
.0859 
1.0911 
1.0964 
1.1018 

21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
24 
35 
36 
37 
38 
39 
40 

1.1071 
1.1125 
1.1179 
1  .  1234 
1  .  1289 
1  .  1344 
1.1399 
1.1454 
1.1510 
1  .  1566 
1  .  1622 
1  .  1679 
1  .  1736 
.1793 
1  .  1850 
1  .  1908 
1  .  1965 
1.2023 
1.2082 
1.2140 

(Kohlrausch,  W.  Ann.  1879.  1.) 

Sp.  gr.  of  MgSO4+Aq  at  0°.    S  =pts.  MgSO4 
in  100  pts.  solution. 

S                  Sp.  gr. 

S 

Sp.  gr. 

13.800         1.1586 
11.7458       1.1329 
9.6218       1.1072 

7.4046 
5.0447 
2.5907 

1.0826 
1.0557 
1.0284 

(Charpy,  A.  ch.  (6)  29.  26.) 

Sat.  MgSO4+Aq  boils  at  105°  (Griffiths); 
108.4°  (Mulder). 
Crust  forms  at  103.5°  (solution  containing 
48.4  pts.  MgSO4  to  100  pts.  H2O);  highest 
temp,  observed,  105°.     (Gerlach,  Z.  anal.  26. 
426.) 

B.-pt.  of  MgSO4+Aq  containing  pts.  MgSO4 
to  100  pts.  H2O. 

(Oudemans,  Z.  anal.  7.  419.) 
Sp.  gr.  of  MgSO4+Aq  at  15°. 

Pts. 
B-'pt<     MgSO4     B<"pt- 

Pts.        R 
MgS04     B'~ 

Pts. 
pt-      MgS04 

%  MgSO4 

Sp.  gr. 

%  MgS04 

Sp.  gr. 

100.5°     8.8     102.5° 
101.0     16.7     103.0 
101.5     23.5     103.5 
102.0     29.5     104.0 

34.7     104.5°    51.3 
39.5     105         54.6 
43.8     108         75(?) 
47.7       

1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 

1.01031 
.02062 
.03092 
.04123 
.05154 
.06229 
.07304 
.08379 
.09454 
.  10529 
1.11668 
1  .  12806 
1  .  13945 

14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
25.248 

1, 

.  15083 
.  16222 
.  17420 
18618 
19816 
21014 
22212 
23465 
24718 
25972 
27225 
28478 
28802 

(Gerlach,  Z.  anal.  26.  432.) 
Sp.  gr.  of  MgSO4+Aq  at  9.5°. 

Mass  of  salt  per  unit 
mass  of  solution 

Density  of  solution 
(g.  per  cc). 

0.00191 
0.00380 
0.00569 
0.00758 
0.01132 

.00170 
.00346 
.00526 
.00705 
.01060 

(Gerlach,  Z.  anal.  8.  287.) 

Sp.  gr.  of  MgSO4+Aq  at  23.5°.     a  =  no.  of 
3/2  mols.  in  grms.  dissolved  in  1000  g. 
H2O;  b  =sp.  gr.  if  a  is  MgSO4+7H2O,  ^ 
mol.  wt.  =  123;  c^sp.  gr.  if  a  is  MgSO4, 
Yz  mol.  wt.  =60. 

(McGregor,  C.  N.  1887,   56.6.) 
Sp.  gr.  of  MgSO4+Aq  at  25°. 

Concentration  of  MgSO4 

+Aq 

Sp.  gr. 

1  —  normal 

Vr-       " 
Vr-       " 
Vr-      " 

1.0584 
1.0297 
1.0152 
1.0076 

a               b               c 

a               b 

c 

1        1.056    1.059 
2        1.103    1.114 
3        1.141    1.166 
4        1.174    1.214 

5        1.203 
6        1.229 
7        1.252 
8        1.273 

1.260 

(Wagner,  Z.  phys.  Ch.  1890,  5.  38.) 

Sp.  gr.  at  16°/4°  of  MgSO4+Aq  contain- 
ng    11.0222%   MgSO4  =  1.1  1471;    containing 
8.343%    MgSO4  =  1.08558.      (Schonrock,    Z. 
phys.  Ch.  1893,  11.  782.) 

(Favre  and  Valson,  C.  R.  79.  968.) 

SULPHATE,  MAGNESIUM 


987 


Sp.  gr.  of  MgSO4+Aq. 

Sp.  gr.  of  MgSO4+Aq  at  20°. 

G.  -equivalents 
MgSO4  per  liter 

t° 

Sp.  gr.  t°/t° 

Normality  of            m   A/r  ork 
MgS04+Aq              %  MgS°4 

Sp.  gr. 

0.002548 
0.005093 
0.01015 
0.02023 
0.05023 
0.09950 
0.19773 
0.29459 
0.48671 

17.989 
18.020 
17.995 
17.980 
18.047 
18.033 
18.014 
17.997 
17.994 

1.0001625 
1.000324 
1.000639 
1.001274 
1.003117 
1.006122 
1.012035 
1.017806 
1.029101 

2.73                  25.46 
1.86                   18.61 
0.934                 10.14 

1.2879 
1.2019 
1  .  1049 

(Forchheimer,  Z.  phys.  Ch.  1900,  34.  24.) 

Sp.  gr.  of  dil.  MgSO4+Aq  at  20.004°. 
Conc.  =  g.  equiv.  per  1.  at  20.004°. 
Sp.  gr.  compared  with  H2O  at  20.004°  =  1  . 

0.5022 
5.0220 

17.90 
17.95 

1.03000 
1.26970 

Cone. 

Sp.  gr. 

0.0000                        1 
0.0001                        1 
0.0002                        1 
0.0003                        1 
0.0004 
0.0005 
0.0010                        1 
0.0020 
0.0050 
0.0100 

.000,000,0 
.000,006,4 
.000,012,9 
.000,019,4 
.000,025,9 
.000,032,4 
.000,064,8 
.000,129,4 
.000,322,4 
.000,642,1 

0.002616 
0.005230 
0.01042 
0.02077 
0.12462 
0.24567 

14.096 
14.109 
14.098 
14.092 
14.199 
14.092 

1.0001672 
.0003311 
.000659 
.001306 
.007682 
.014980 

(Kohlrausch,  W.  Ann.  1894,  63.  27.) 
Sp.  gr.  of  MgSO4+Aq. 

(Lamb  and  Lee,  J.  Am.  Chem.  Soc.  1913.  36. 
1684.) 

More  sol.  in  HCl+Aq  than  in  H2O.    (Rich- 
ter.) 
In   sat.    HCl+Aq,    anhydrous    MgSO4    is 
scarcely  sol.;  MgSO4+7H2O  dissolves,  but  is 
precipitated  by  a  current  of  HC1  gas.    (Hens- 
gen,  B.  10.  259.) 
Margueritte  (C.  R.  43.  50)  denies  the  pre- 
cipitation. 
For  solubility  in  H2SO4,  see  MgH2(SO4)2. 
Completely    pptd.    from    MgSO4+Aq   by 
cone.  HC2H3O2+Aq.     (Persoz.) 
Somewhat  sol.   in   sat.   NH4Cl+Aq  with 
separation  of  a  double  sulphate. 
^  Rapidly  sol.  in  KCl+Aq  with  separation  of 
K2SO4. 
Sol.  in  sat.  NaCl+Aq  without  pptn.  of  the 
latter. 
Easily  sol.  in  sat.  KNO3+Aq  without  caus- 
ing any  pptn. 
Sol.  in  sat.  NaNO3+Aq.    (Karsten.) 
Rapidly    sol.    in    sat.    CuSO4+Aq;    when 
saturation  is  reached,  a  double  salt  separates 
out.    (Karsten.) 
100  pts.  sat.  MgSO4+NiSO4+Aq  at  18-20° 
contain  30.93  pts.  of  the  two  salts;  100  pts. 
sat.  MgSO4+ZnSO4+Aq  at  18-20°  contain 
35.45  pts.;   100  pts.   sat.   MgSO4+NiSO4  + 
ZnSO4+Aq  at  18-20°  contain  35.62  pts.  (v. 
Hauer,  J.  pr.  98.  137.) 
100  pts.  H2O  dissolve  14.1  pts.  MgSO4  and 
9.8  pts.  K2SO4,  if  sat.  MgSO4+Aq  is  sat.  with 
K2SO4;  32.4  pts.  MgSO4  and  8.2  pts.  K2SO4, 
if  sat.  K2SO4+Aq  is  sat.  with  MgSO4.  all  at 
15°.    (Mulder.  J.  B.  1866.) 
100  pts.  H2O  dissolve  25.95  pts.  MgSO4  and 
5.21  pts.  Na2SO4  at  0°.    (Diacon,  J.  B.  1866. 
62.) 

1A  MgSO4  g.  in  1000  g. 
of  solution 

Sp.  gr.  16°/16° 

0 
0.5368 
1.0917 

2.1076 
4.1367 
9.0608 
18.0846 
37.1342 
52.1362 

1.000000 
1.000570 
1.001157 
1.001141 
1.002234 
1.004372 
1.009523 
1.018954 
1.038983 
1.054867 

(Dijken,  Z.  phys.  Ch.  1897,  24.  108.) 

Sp.  gr.  of   MgSO4+Aq  at  18.2°,  when  p  = 
per  cent  strength  of  the  solution;  d  = 
observed  density;  and  w  =  volume  cone. 

in  grams  per  cc.  /  JQQ  =  w.  ) 

p 

d 

w 

26.25 
25.91 
24.53 
21.60 
18.41 
13.79 
12.63 
11.29 
8.08 
2.01 

.2903 
.2860 
.2693 
.2330 
.1950 
.1423 
.1291 
1.1147 
1.0803 
1.0204 

1.3374 
1.3319 
.3101 
.2650 
.2187 
.1562 
.1413 
.1246 
.0859 
.0191 

(Barnes,  J.  phys.  Chem.  1898,  2.  542.) 

988 


SULPHATE,  MAGNESIUM  HYDROGEN 


100  pts.  H2O  dissolve  15.306  pts.  MgSO4 
and  13.086  pts.  Na2SO4  at  0°.     (Pfaff,  A.  99. 

224.) 

See  also  under  MgNa2(SO4)2+4H2O. 

Solubility  of  mixtures  of  MgSO4  and 
MgNa2(SO4)2+4H2O  at  t°. 


t° 

g.  per  100  g.  H2O 

Na2SO4 

MgSO4 

22 
,  24.5 
30 
35 

23.3 

27.2 
36.1 
33.9 

31.4 
24.2 
19.1 
18.44 

(Roozeboom,    1888,   Z.    phys.   Ch.   2.  "518.) 
See  also  under  MgNa2(SO4)2+4H2O. 

Slowly  sol.  in  sat.  ZnSO4+Aq  without  pptn. 
until  saturation,  when  a  double  salt  separates 
out. 

Insol.  in  liquid  NHs.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

100  pts.  dil.  alcohol  containing  at  15°: 

10        20        40  %  alcohol 

contain  39 . 3    21 . 3     1 . 62%  MgSO4+7H20. 

(Schiff,  A.  118.  365.) 

At  higher  temp,  the  solubility  increases 
proportional  to  the  temp.  (Gerardin,  A.  ch. 
(4)  5.  145.) 

103  pts.  absolute  methyl  alcohol  dissolve 
1.18  pts.  MgSO4  at  18°.  (de  Bruyn,  Z.  phys. 
Ch.  10.  783.) 

100  pts.  absolute  methyl  alcohol  dissolve 
41  pts.  MgSO4+7H2O  at  17°;  100  pts.  abso- 
lute methyl  alcohol  dissolve  29  pts.  MgSO4+ 
7H2O  at  3-4°;  100  pts.  93%  methyl  alcohol 
dissolve  9.7  pts,  MgSO+7H2O  at  17°;  100 
pts.  50%  methyl  alcohol  dissolve  4.1  pts. 
MgSO4+7H2O  at  3-4°.  (de  Bruyn,  R.  t.  c. 
11.  112.) 

100  pts.  absolute  ethyl  alcohol  dissolve  1.3 
pts.  MgSO4+7H2O  at  3°.  (de  Bruyn.) 

Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.  257.) 

Insol.   in   methyl   acetate    (Naumann,    B. 

1909,  42.  3790.);  ethyl  acetate  (Naumann,  B. 

1910,  43.    314.);   acetone.     (Naumann,    B. 
1904,  37.  4329.) 

100  g.  95%  formic  acid  dissolve  0.34  g. 
MgSO4  at  19°.  (Aschan,  Ch.  Ztg.  1913,  37. 
1117.) 

100  g.  sat.  solution  of  MgSO4  and  sugar 
in  H2O  contains  46.52.  g.  sugar  +14.0  g. 
MgSO4,  or  100  g.  H2O  dissolve  119.6  g.  sugar 
+36.0  g.  MgSO4.  (Kohler,  Z.  Ver.  Zucker- 
ind,  1897,  47.  447.) 

Magnesium  hydrogen  sulphate,  MgH2(SO4)2. 
Decomp.  by  H2O.     Sol.  in  H2SO4.     Insol. 
in  methyl  acetate.     (Naumann,  B.  1909,  42. 
3790.) 


MgH6(SO4)4.  Boiling  H2SO4  dissolves 
about  2%  MgSO4,  from  which  this  compound 
crystallises.  (Schultz,  Pogg.  133.  137.) 


Magnesium  p?/rosulphate,  MgS20  7. 
Decomp.  by  H2O. 


Magnesium   manganous  sulphate, 

2MnSO4  +  15H2O. 
Min.  Fauserite. 


MgS04, 


Magnesium  manganous  zinc  sulphate,  MgS04, 

MnSO4,  ZnSO4+21H2O. 
Sol.  in  H2O.    (Vohl,  A.  99.  124.) 

Magnesium  nickel  sulphate,  MgSO4,  3NiSO4 

+28H2O. 
Sol.  inHaO.    (Schiff.) 

Magnesium  nickel  potassium  sulphate, 

MgSO4,  NiSO4,  2K2SO4+12H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 

Magnesium  potassium  sulphate, 

MgK2(SO4)2+6H2O. 
100  pts.  H2O  dissolve  22.7  pts.  anhydrous 
salt  at  16.5°.    (Mulder.) 

100  pts.  H2O  dissolve  at: 
0°        10°       20°       30°       35° 
14.1     19.6    25.0    30.4     33.3    pts.    anhy- 
drous salt, 

45°       55°      60°       65°       75° 
40.5     47.0     50.2     53.0     59.8   pts.    anhy- 
drous salt. 
(Tobler,  A.  95.  193.) 

100  g.  H2O  dissolve  30.52  g.  MgK2(SO4)2  + 
6H2O  at  15°.  (Lothian,  Pharm.  J.  1909,  82. 
292.) 

Solubility  in  H2O  at  t°. 


Sat.  solution 
contains 

Mols. 
K2S04: 

100  pts.  H20 
dissolve 

t° 

mo  Is. 

K2§04 

MgS04 

the  solu- 
tion 

K2S04 

MgSO4 

10 

9.4 

9.8 

1:   .52 

11.63 

12.13 

20 

10.9 

10.8 

1:   .43 

13.92 

13.79 

30 

12.4 

11.8 

1:   .38 

16.36 

15.56 

40 

13.8 

13.1 

1:   .37 

18.88 

17.92 

50 

14.7 

14.8 

1:   .46 

20.85 

20.99 

60 

15.2 

16.3 

1:   .55 

22.19 

23.79 

70 

15.6 

16.8 

1:1.52 

23.07 

24.85 

80 

16.0 

17.1 

1:1.56 

23.91 

25.56 

80 

16.6 

18.1 

1:1.58 

25.42 

27.72 

90 

17.2 

18.2 

1:1.54 

26.62 

28.17 

(Precht,  B.  1882,  15.  1668.) 


SULPHATE  POTASSIUM  CHROMATE,  MAGNESIUM 


Sp.  gr.  of  aqueous  solution  at  15°  contain- 

100 mols.  H2O  hold  mols.  salt  in  solution 

ing: 

at  t°. 

2             4             6             8%  hydrous  salt, 
1.0129    1.0261    1.0394    1.053 

t° 

MgSO4 

Na2SO4 

10          12            14           16%  hydrous  salt, 
1.0668    1.0808    1.095      1.1094 

22 
24.5 
30 

4.70 
3.68 
3.60 

2.95 
3.45 
3.60 

18           20             22%    hydrous  salt. 
1  .  124      1  .  1388      1  .  1539 

35 

47 

3.69 
3.60 

3.69 
3.60 

(Schiif,  A.  113.  183,  calculated  by  Gerlach, 

(Roozeboom,  R.  t.  c.  1887,  6.  333.) 

Z.  anal.  8.  287.) 

Sp.  gr.  of  MgK2(S04)2+Aq  at  18°. 

Solubility    of    mixtures    of 
4H2O  and  Na2SO4 

MgNa2(S04)2  + 
at  t° 

G-equiv.  of  salt  per  1. 

Sp.  gr. 

g.  per  100  g.  H2O 

1.0010 

1.0633 

t° 

0.8345 

1.0531 

Na2SO4 

MgSO4 

0.6688 
0.3744 
0.0998 
0.02004 
0.01004 

1.0427 
1.0243 
1.0040 
1.0015 
1.0004 

18.5 
22 
24.5 
30 
35 

43.0 
35.2 
32.5 
25.9 
23.5 

45.5 
48.9 
50.3 
55.0 
59.4 

These  results  lead  the  author  to  conclude 
that  in  dil.  solutions  the  double  salt  is  de- 
comp.  into  its  constituents.  (McKay,  Elek- 
trochem.  Zeit.  1899,  6.  115.) 

Min.  Picromerite. 

+4H2O.      (van   der   Heide,   B.   26.   414.) 

2MgSO4,  K2SO4.     Min.  Langbeinite. 

Deliquescent.  Absorbs  56.26%  H2O  from 
air  to  form  K2SO4,  MgSO4+6H2O.  (Mallet, 
Chem.  Soc.  1900,  77.  220.) 

4MgSO4,  K2SO4+5H2O.  (van't  Hoff  and 
Kassatkin,  B.  A.  B.  1889.  951.) 

Magnesium  potassium  zinc  sulphate,  MgSO4, 

2K2SO4,  ZnSO4  +  12H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  57.) 

Magnesium    potassium    sulphate    chloride, 

MgSO4,  K2SO4,  MgCl2+6H2O. 
Min.  Kainite. 

Magnesium     rubidium     sulphate,     MgSO4, 

Rb2SO4+6H2O. 

Sol.  in  H2O.    (Tutton,  Chem.  Soc.  63.  337.) 
1  1.  H2O  dissolves  202  g.  anhydrous  salt 

at  25°.    (Locke,  Am.  Ch.  J.  1902,  27.  459.) 
2MgSO4,  Rb2SO4.    Deliquescent.     (Mallet, 

Chem.  Soc.  1900,  77.  223.) 

Magnesium  sodium  sulphate,  MgSO4,  Na2SO4 
+4H20. 

Min.  Blodite  t  Simonyite. 

Blodite  is  efflorescent;  Simonyite,  deli- 
quescent. 

+5H2O.    Min.  Louriie. 

-j-6H2O.  Decomp.  on  air.  Sol.  in  3  pts. 
cold  H2O. 

Na6Mg(SO4)4.  Min.  Vanthoffite.  (van't 
Hoff,  B.  A.  B.  1902.  414.) 

MgNa2(SO4)2+4H2O.    Min.  Astrakanite. 


(Roozeboom,   Z.   phys.    Ch.    1888,    2.   518.) 
See  also  under  MgSO4. 

Magnesium  thallous  sulphate,  MgSO4,  T12SO4 

+6H2O. 

Sol.  in  H2O,  but  decomp.  by  repeated  re- 
crystallisations.    (Werther.) 


Magnesium  uranyl  sulphate, 

MgSO4,  (UO2)SO4+5HO2. 
(de  Coninck,  Chem.  Soc.  1905, 


J.  (2)  530.) 


Magnesium  zinc  sulphate,  MgSO4,  ZnSO4  + 
14H2O. 

Sol.  in  H2O.     (Pierre,  A.  ch.  (3)  16.  244.) 

+  10H2O.     (Pierre.) 

3ZnSO4,  5MgSO4+56H2O.    (Schiff.) 

There  are  only  two  compounds,  2(MgSO4> 
7H2O),  ZnSO4,  7H2O  and  MgSO4,  7H2O, 
ZnSO4.  7H2O.  (Hollmann,  Z.  phys.  Ch. 
1901,  37.  212,  and  1902,  40.  577. 

Magnesium  sulphate  potassium  chloride, 
MgSO4,  KC1+3H2O  or  MgSO4,  K2SO4, 
MgCl2+6H2O. 

Min.  Kainite. 

100  pts.  H2O  dissolve  79.56  pts.  at  18°. 
(Krause,  Arch.  Pharm.  (3)  6.  326.) 

Not  sol.  in  a  mixture  of  abs.  alcohol  and 
ether,  which  dissolves  out  MgCl2.  (Lehmann, 
J.  B.  1867.  416.) 

Alcohol  dissolves  out  MgCl2,  also  little 
H2O.  Much  H2O  dissolves  completely. 
(Zincken,  Miner.  Jahrb.  1866.  310.) 

Magnesium  sulphate  potassium    chromate, 

2MgSO4,  K2CrO4+9H2O. 
Sol.  in  H2O.    (fitard,  C.  R.  86.  443.) 


990 


SULPHATE,  MANGANOUS,  BASIC 


Manganous  sulphate,  basic,  3MnO.  2SO3+ 
3H2O. 
Insol.  in  H2O,  but  slowly  decomp.  therebv. 
(Gorgeu,  C.  R.  94.  1425.) 

Manganous  sulphate,  MnSO4. 

Anhydrous. 

Absorbs  H2O  from  the  air  to  form  MnSO4+4H2O. 
l.pt.  MnSO4  is  sol.  in  pts.  H2O  at  t°. 

100    pts.  H2O    dissolve    pts.    MnSO4    from 
MnSO4+H2O  at  t°. 

t° 

Pts. 
MnSO4 

t° 

Pts. 
MnSO4 

Pts. 
MnSO4 

48 
53 
65 

72 

87.98 
86.10 
84.33 

82.73 

78 
90 
100 
106 

79.13       1 
75.63       1 
71.27 
70.14 

15      69.78 
17      68.81 

t 

Pts. 

H20 

t° 

Pts. 
H2O 

t 

Pts. 
H20 

(Linebarger.) 
Min.  Szmikite. 

Solubility  of  MnSO4+H2O  in  H2O  at  t°. 

6.25 
10 

1.77 
1.631 

18.75 
37.5 

1.667 
T457 

75 
101.25 

1.494 
2.031 

Or— 
100  pts.  H2O  dissolve  pts.  MnSO4  at  t°. 

t° 

Pts. 
per 

MnSO4 
100  pts. 
H20 

t° 

Pts.  MnSO4 
per  100  pts. 
H20 

t 

6.25 
10 

Pts. 
MnS04 

t 

Pts. 
MnSO4 

t° 

Pts. 
MnS04 

41. 
50. 
67. 

5 
1 
1 

61.06 
58.01 
51.37 

75 
84.8 
95 
99.6 

49.45 

44.87 
38.71 
34.27 

56.49 
61.29 

18.75 
37.5 

60.00 
68.63 

75 

101.25 

66  .  95 
49.33 

(Brandes,  Pogg.  20.  575.) 

Sol.  in  2.5  nts     H^O  at   18  75°  •   nt  (\9  Z0  it  i«  rliffir-iilt 

to  dissolve  1  pt.  MnSO4  in  3  pts.  H2O,  but  the  sat. 
solution  at  62.5°  does  not  become  cloudy  on  heating 
to  100°.  (Jahn.) 

100  pts.  MnSO4+Aq  sat.  at  11-14°  contain 
37.5  pts.  MnSO4.  (v.  Hauer,  J.  pr.  103.  114.) 

Sat.  MnSO4+Aq  contains  at: 
—8°  —5°     +5°   18°     22° 

30.0  31.0    34.1  38.3  38.2%  MnSO4, 

23°     32°      45°     52°     70° 

39.1  41.7    44.2  36.4  41.1%MnSO4, 

83°     110°    115°  123°   130°   140° 
36.3  18.4   21.5  16.7  13.6  9.4%  MnSO4. 
(Etard,  A.  ch.  1894,  (7)  2.  553.) 

Solubility  in  H2O  increases  from  0-55°,  and 
decreases  from  55-145°.  The  increasing  solu- 
bility is  that  of  MnSO4+5H2O,  and  MnSO4  + 
2H2O  separates  out  at  35°,  and  is  completely 
insol.  at  145°.  (fitard.) 

If  solubility  S=pts.  anhydrous  MnSO4  in 
100  pts.  solution,  S  =  30.0+0.2828t  from  —8° 
to  57°;  S  =48.0-0.4585t  from  57°  to  150°. 

Practically  insol.  in  H2O  at  180°.  (fitard, 
C.  R.  106.  208.) 

Solubility  varies  according  to  the  hydrate 
used.  Above  results  of  Etard  show  the  solu- 
bility of  MnSO4+7H2O  at  0°,  and  MnSO4  + 
3H2O  at  57°.  Anhydrous  MnSO4  is  stable 
only  above  117°.  (Linebarger.) 

100  pts.  H2O  dissolve  pts.  anhydrous  MnSO4 
att°. 


t° 

Pts. 
MnS04 

t 

Pts. 
MnS04 

t° 

Pts. 
MnSO4 

120 
132 

67.18 
63.16 

141 
146 

41.18 

38.83 

155 
170 

26.49 
16.15 

(Linebarger,  Am.  Ch.  J.  15.  225.) 
+H2O.    Stable  only  between  57°  and  117C 


Av.  of  varying  results. 

(Cottrell,  J.  phys.  Ch.  1900,  4.  652.) 

Linebarger's  determinations  are  inaccurate. 
(Cottrell.) 

+2H2O.    Stable  between  40°  and  57°. 


100  pts.  H2O  dissolve  pts.  MnSO4  from 
MnSO4+2H2O  at  t°. 


t° 

Pts. 
MnSO4 

t° 

Pts. 
MnSO4 

t° 

Pts. 
MnSO4 

35 

40 

68.88 
75.31 

42 
45 

77.63 
80.07 

50 

55 

83.16 

86.27 

(Linebarger.) 
-f  3H2O.    Stable  between  30°  and  40°. 

100  pts.  H2O  dissolve  pts.  MnSO4  from 
MnSO4+3H2O  at  t°. 


t° 

Pts. 
MnS04 

t° 

Pts. 
MnSO4 

t 

Pts. 
MnSO4 

5 
12 
16 
19 

54.68 
60.56 
63.41 
65.12 

25 
30 
35 
40 

66.85 
67.38 
68.31 
70.63 

68 
53 
57 

71.89 
72.81 
73.17 

(Linebarger.) 

+4H2O.    SI.  efflorescent.    Less  sol.  in  boil- 
ing than  in  cold  H2O. 
100  pts.  H2O  at  4.4°  dissolve  31  pts.  MnSO4 
+4H2O.     (Jahn.) 

SULPHATE,  MANGANOUS 


991 


100  pts.  H2O  at  t°  dissolve  pts.  MnSO4+4H2O. 

Solubility  of  MnSO4+4H2O  in  H2O  at  t°. 

Pts. 
t°                MnSO4  + 
4H20 

t°  % 

Pts. 
MnSO4  + 
4H2O 

Pts.  MnSO4 
t°              per  100  pts. 
H20 

t° 

Pts.  MnSO4 
per  100  pts. 
H20 

6.25               113.22 
10                     123 
18.75               122 

37.5 
75 
101.25 

149 
144 
93 

16.0           63.97 
17.7           64.16 
18.5           64.19 
25.0           65.32 
30.0           66.43 
32.2           66.83 

35.0 
35.5 
39.9 
49.9 
50.0 

67.87 
68.09 
68.81 
72.48 
72.62 

(Brandes,  Pogg.  20.  575.) 

Solubility  of  MnSO4  in  100  pts. 
using  MnSO4+4H2O. 

H2O  at  t°, 

t° 

Pts. 
MnSO4 

t° 

Pts. 
MnSO4 

t° 

Pts. 
MnS04 

(Cottrell,   J.   phys.   Ch.    1900,  4.   651.) 

Linebarger's    determinations   are    inaccu- 
rate.    (Cottrell.) 

Solubility  in  H2O  at  t°. 

0 
1 
2 
3 
4 
5 
6 
.      7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
34 

55.4 
55.9 
56.5 
57.1 
57.7 
58.2 
58.8 
59.4 
60.0 
60.5 
61.1 
61.7 
62.2 
62.7 
63.3 
63.8 
64.3 
64.8 
65.3 
65.8 
66.3 
66.7 
67.2 
67.6 
68.1 
68.5 
68.9 
69.3 
69.7 
70.0 
70.4 
70.7 
71.0 
71.3 
71.6 

35 

36 
37 
38 
39 
40 
41 
42 
43 
44 
45 
46 
47 
48 
49 
50 
51 
52 
53 
54 
55 
56 
57 
58 
59 
60 

63.5 
64 
65 
66 
67 
68 
69 

71.9 

72.2 
72.4 

72.7 
72.9 
73.1 
73.3 
73.5 
73.7 
73.9 
74.0 
74.2 
74.4 
74.6 
74.7 
74.8 
74.9 
75.1 
75.2 
75.3 
74.7 
74.0 
72.9 
71.5 
69.5 
65.9 

61.'3 
61.5 
61.5 
61.5 
61.5 
61.5 
61.5 

70 
71 

72 
73 
74 
75 
76 
77 
78 
79 
80 
81 
82 
83 
84 
85 
86 
87 
88 
89 
90 
91 
92 
93 
94 
95 
96 
97 
98 
99 
100 
101 
102 
102.5 

61.5 
61.5 
61.5 
61.5 
61.5 
61.5 
61.5 
61.5 
61.5 
61.5 
61.5 
61.5 
61.5 
61.5 
61.4 
61.3 
61.2 
61.0 
60.8 
60.6 
60.3 
60.0 
59.6 
59.2 
58.6 
57.9 
57.2 
56.3 
55.4 
54.3 
52.9 
51.2 
49.3 
47.4 

t° 

g.  MnSOi  for  100  g.  H2O 

30.15 
35 

66.38 
68.22 

(Richards  and  Fraprie,  Am.  Ch.  J.  1901,  26. 

77.) 

+5H2O.     Sol.    in    1    pt.    H2O   at    18.75°. 
(Jahn,  A.  28.  110.) 
Stable  from  8°  to  18°. 

100  pts.  H2O  dissolve  pts.  MnSO4  from 
MnSO4+5H2O  at  t°. 

fo                  PtS.                    ,o 

MnS04 

Pts. 
MnS04 

t° 

MnSO4 

0        58.05        20 
2.5     62.41        25 
4        64.22        30 
7         66.83        32 
10        68.05        34 
15         72.33        37 

75.16 
78.63 
79.16 
80.38 
82.04 
83.91 

40        84.63 
42        85.27 
45        86.16 
47.7     86.95 
53        88.89 
54        89.08 

(Linebarger.) 

Stable  in  aqeous  solution  between  15°  and 
20°.    (Schieber,  M.  1898,  19.  281.) 

Solubility  of  MnSO4+5H2O  at  t°. 

(Mulder,  Scheik.  Verhandel.  1864.  137. 

100  pts.  H2O  dissolve  pts.  MnSO4  from 
MnSO4+4H2O  at  t°. 

Pts.  MnSO4 
t°             per  100  pts. 
H20 

t° 

Pts.  MnSCU 
per  100  pts. 
H20 

t° 

2.2 
7.3 
11 
15 
20 

Pts. 
MnS04 

t° 

Pts. 
MnS04 

t° 

Pts. 
MnSO4 

57.88 
61.78 
64.01 
67.12 
69.93 

25 
30 
35.5 
40 
45 

72.23 
74.67 

78.81 
79.63 
83.06 

48 
52 
56 

84.33 
86.16 
88.19 

5               58.06 
9               59.23 
12               60.19 
12.3           60.16 
15               61.08 

16 
25 
30 
31.1 
35.5 

61.59 

64.78 
67.76 
67.92 
71.61 

(Linebarger.) 

Stable  in  aqueous  solution  between  25°  and 
31°.    (Schieber,  M.  1898,  19.  281.) 

(Cottrell,  J.  phys.  Ch.  1900,  4.  651.) 

Linebarger's  determinations  are  inaccurate. 
(Cottrell.) 

992 


SULPHATE,  MANGANOUS 


Solubility  in  H2O  at  25°  =65.09  g.   MnSO4 

Sp.  gr.  of  MnSO4+Aq  at  15°. 

for  100  g.  H2O.    (Richards  and  Fraprie,  Am. 

Ch.  J.  1901,  26.  77.) 

%  MnSCU 
+4H20 

Sp.  gr. 

%  MnS04 
+4H20 

Sp.  gr. 

+6H2O.    Stable  from-  5°  to  +8°. 

1 

1.006 

29 

1.208 

100  pts.  H2O  dissolve  pts.  MnSO4  from 
MnSO4+6H2O  at  t°. 

2 
3 
4 

1.013 
1.020 
1.025 

30 
31 
32 

1.2150 
.224 
.231 

t° 

Pts. 

Pts. 

Pts. 

5 

1.0320 

33 

.244 

t 

MnSO4 

t 

MnS04 

t 

MnSO4 

6 

71 

1.038 

1f\A  A 

34 

O  C 

.250 

oc^rri 

—  4 

55.87 

9 

70.88 

30 

76.24 

8 

.U44 

1.050 

65 
36 

.2579 

.268 

0 

64.21 

15 

72.45 

34 

77.02 

9 

1.056 

37 

1.276 

3 

66.87 

20 

74.35 

35 

77.23 

10 

1.0650 

38 

1.285 

5 

67.49 

25 

75.38 

38 

7.481 

11 
i  n 

1.072 

1    H7Q 

39 

Af\ 

1.295 

1OPIQQ 

(Linebarger.) 

iz 
13 
14 

i  .u/y 
1.085 
1.093 

4U 

41 
42 

.oUoo 

1.313 
1.322 

15 

1  .  1001 

43 

1.331 

16 

1.106 

44 

1.340 

+7H2O.     Efflorescent. 

17 

.114 

45 

.3495 

Sol.  in  less  than  0.5  pt,  H2O  at   18.75°. 

18 

.121 

46 

.360 

(Jahn.) 

19 

.129 

47 

.370 

Stable  between  -  10°  and  -  5°. 

20 

.1363 

48 

.380 

21 

.144 

49 

.389 

22 

.150 

50 

.3986 

100  pts.  H2O  dissolve  pts.  MnSO4  from 
MnSO4+7H2O  at  t°. 

23 

24 
25 

O£» 

.160 
1.166 
1.1751 

1     1  Q'i 

51 
52 
53 

1.410 
1.420 
1.430 

1    AA.f\ 

t° 

Pts. 
MnS04 

t° 

Pts. 
MnSO4 

t° 

Pts. 
MnSO4 

^O 

27 
28 

I  .  loo 

1.190 
1.200 

: 

55 

1  .'±4U 

1.4514 

50.11 

0 

53.61 

10 

59.91 

—  10 

-8 

50.93 

5 

54.83 

15 

64.34 

(Gerlach,  Z.  anal.  8.  288.) 

—5 

51.53 

7 

56.62 

(Linebarger.) 


Stable    in    aqueous    solution    below    Oc 
(Schieber,  M.  1898,  19.  281.) 


Solubility  of  MnSO4+7H2O  in  H2O  at  t°. 


Sp.  gr.  of  MnSO4+Aq  at  23°.  a=no.  of  ^ 
mols.  in  grms.  dissolved  in  1000  g.  H2O; 
b=sp.  gr.  if  a  is  MnSO4+5H2O,  K  mol. 
wt.  =  120.5;  c  =  sp.  gr.  if  a  is  MnSO4, 
V>  mol.  wt.  =75.5. 


t 

Pts.  MnSO4 
per  100  pts. 
H20 

t° 

Pts.  MnSO4 
per  100  pts. 
H20 

—  10 
0 
5 

47.96 
56.23 
56.38 

9 
12 
14.3 

59.33 
61.78 
63.93 

a 

b 

c 

a 

b 

c 

1 

2 

3 
4 
5 

1.068 
1.128 
1.181 
1.227 
1.269 

1.071 
1.139 
1.202 
1.262 
1  .320 

6 
7 
8 
9 
10 

1.306 
1.341 
1.371 
1.399 
1.426 

3.576 
1.429 

(Cottrell,  I.  c.) 


M.-pt.  of  MnSO4+7H2O  is  54°.     (Tilden, 
Chem.  Soc.  46.  409.) 


(Favre  and  Valson,  C.  R.  79.  968.) 


Above  table  recalculated  by  Gerlach  (Z.  anal. 
28.  475.) 


%  MnSO4 
+5H2O 

Sp.  gr. 

%  MnS04 
+5H20 

40 
50 

Sp.  gr. 

1.2900 
1.3800 

10 
20 
30 

1.0630 
1  .  1325 
1.2070 

SULPHATE,  MANGANOUS 


993 


Sp.  gr.  of 

MnSO4+Aq  at  15°.    a  =  %;  b  = 

Sol.  in  about  20  pts.  boiling  H2SO4,  and 

sp.  gr.  if  a  is  MnSO4;  c  =  sp.  gr.  if  a  is 
MnSO4+4H2O;  d  =  sp.  gr.  if  a  is  MnSO4 
+5H2O;    e  =  sp.    gr.    if   a   is    MnSO4+ 

more  sol.  in  boiling  H2SO4+Aq  of  1.6  sp.  gr. 
(Schultz,  Pogg.  133.  137.) 
Completely  pptd.  from  solution  by  HC2H3O2. 

7H2O. 

(Persoz.) 

b 

•  c 

For  solubility  in    (NH4)2SO4,   see   under 

a 

d 

e 

(NH4)2S04. 

5 
10 
15 

1.0500 
.1035 
.1605 

1.0340 
1.0690 
1  .  1055 

1.0310 
1.0630 
1.0965 

1.0270 
.0545 
.0830 

MnSO4+Aq   sat.  at  10°,    then   sat.   with 
K2SO4  at  same  temp,  contains  for  100  pts. 
H2O  16.7  pts.    MnSO4  and  44.3  pts.    K2SO4 
(IVTiilcl.Gr  ^ 

20 

.2215 

1  .  1435 

1.1315 

.1130 

25 

.'2870 

1  .  1835 

1  .  1685 

.1440 

30 

.3575 

1.2255 

1.2070 

.1765 

35 

1.2695 

1.2470 

.2105 

Solubility  of  MnSO4+Na2SO4  in  H2O  at  35°. 

40 

1.3155 

1.2885 

.2455 

45 

rr\ 

1.3640 

1.3315 

1.2815 

g.  per  100  g.  sat.  solution 

50 
55 

.  .  . 

1  .  3760 

1.3185 
1.3565 

MnSCU 

Na2SO4 

Solid  phase 

(Gerlach,  Z.  anal.  28.  475.) 

39.45 
33.92 

0 
5.23 

MnS04,  H20 

Sp.  gr.  of  MnSO4-(-Aq 

at  0°.  S  =  pts.  MnSO4 

33.06 

7.97 

MnS04,  H2O+9MnSO4, 

in 

100  pts 

solution. 

10Na2SO4 

qo  no 

7  42 

n 

S 

Sp.  gr. 

S 

Sp.  gr. 

O&  •  t/£ 

31.05 

1    *  TZA 

9.20 

9MnS04)f10Na2SO4 

16.7450 

1 

1834 

~~ 

5.8295 

1.0928 

27.67 
22.14 

10.76 
14.28 

tt 

14.0462 

1 

1519 

6.0172 

1.0622 

14.58 

20.01 

u 

11.5804 

1 

1239 

3.0865 

1.0315 

13.96 

21.91 

f\*\  fT       C1/"\           -1  *"k"VT         C*/~\         1 

(Charpy,  A.  ch. 

Sp.  gr.  of  MnSO4+Aq 
taming  r 

(6)  29.  26.) 
at  room  temp,  con- 

12.19 

10.45 
7.43 

5fiQ 

22.49 

23.41 
26.58 

OQ    Q1 

9MnSO4,  10Na2SO4+ 
MnS04,  3Na2S04 
MnS04,  3Na2S04 
" 

11.45 
1.1469 

18.8 
1.2513 

22.08  %MnSO4. 
1.3082 

.  D»7 

5.11 
2.96 

£>\J   •   OX 

30.52 
31.33 

MnSO4,  3Na2SO4+Na2SO4 
Na2S04 

(Wagner,  W.  Ann.  1883,  18.  271.) 

0 

33 

Sp. 

gr.  of  MnSO4+Aq  at  25°. 

(Schreinemakers  and  Provije,  Proc.  Ak.  Wet. 

Concentration  of 

+Aq 

MnSO.. 

Sp.  gr. 

Amsterdam,  1913,  16.  326.) 

1—  normal 

1.0728 

Insol.  in  liquid  NH3.     (Franklin,  Am.  Ch. 

v«- 

1  .  0365 

J.  1898,  20.  828. 

1/4  — 

1  1 

1.0179 

Anhydrous   MnSO4  in  insol.   in   absolute 

Vs- 

(t 

1.0087 

alcohol. 

Vie"        " 

1.0041 

1000  pts.  alcohol  of  0.872  sp.  gr.  dissolve 

(Wagner,  Z.  phys. 

Ch.  1890,  6.  39.) 

6.3  pts.  MnSO4. 
Sol.  in  50  pts.  of  50%  alcohol.     Insol.  in 

Sp.  gr.  at  16°/4°  of  MnSO4-f  Aq.  contain- 
ng  30.819%  -MnSO4  =  1.36267.     (Schonrock, 
5.  phys.  Ch.  1893,  11,781.) 

absolute  alcohol.     (Brandes,  Pogg.  20.  556.) 
100  pts.  solution  saturated  at  15°  in  dil. 
alcohol  containing: 

Sat.    MnSO4+Aq   boils   at    102.4°;    crust 
orms  at  101.6°,  and  solution  contains  48.7 

0          10      50        60  %  alcohol,  contain 
56.25    51.4    2.0    0.66  pts.  MnSO4+5H2O. 

>ts.  MnSOj  to  100  pts.  H2O. 

.-pt.  of  MnSO4+Aq  containing  pts.  MnSO4 
to  100  pts.  H2O. 


i     B.-pt. 

Pts.  MnSO4 

B.-pt. 

Pts.  MnSO4 

100.5° 
101.0 
101  .-fr 

17.1 
32.1 
46.2 

102.0° 
102.4 

58.9 
68.4 

(Gerlach,  Z.  anal.  26.  434.) 


(Schiff,  A.  118.  365.) 


When  MnSO4+7H2O  is  boiled  with  ab- 
solute alcohol  none  is  dissolved,  but  MnSO4 
-H3H2O  is  formed. 

When  MnSO4 +7H2O  is  dissolved  in  15-50% 
alcohol,  the  liquid  separates  into  two  layers, 
the  lower  containing  less  (12-14%)  alcohol 
and  more  (47-49%)  salt;  the  upper  containing 


994 


SULPHATE,  MANGANOUS 


more  (50-55%)  alcohol  and  less  (1.3-2.2%) 
salt.  If  the  alcohol  has  the  above  strength 
(15-50%)  the  separation  takes  place  at  ordin- 
ary temp.,  but  with  13-14%  or  60%  or  more 
alcohol,  warming  is  necessary  to  effect  the 
separation.  (Schiff,  A.  118.  363.) 


Solubility  of  MnSO4+H2O  in  alcohol  +Aq 
att°. 


Composition    of    the    solutions    sat.    with 
espect  to  one  another. 


solid 


mpo 
salt 


at  t°. 


30 
31 
35 
37 
41 
42 
43 


Alcohol  layer 


%  alcohol  %  MnSO4 


45.20 
43.90 
41.71 
38.26 
34.01 
32.37 
31.42 


2.49 
2.74 
3.44 
4.84 
5.86 
6.89 
8.51 


Water  layer 


%  alcohol    %  MnSO 


8.69 

8.47 

9.24 

11.03 

11.93 

13.57 

14.33 


30.15 
30.10 
28.61 
26.47 
24.97 
23.09 
22.01 


(Schreinemakers   and   Deuss,    Z.   phys.    Ch 
1912,  79..  559.) 


Composition  of  alcohol  solutions  sat.  with 
MnSO4+H2O  at  t°. 


50 


35 


30 


%  H20 


63.74 
65.21 
65.23 
64.83 
59.41 


61.4 

62.13 

62.06 

62.01 

*62.15 

*54.85 

50.69 

50.16 


61.4 

61.43 

61.25 

60.78 

*61.16 

*52.31 

44.83 

30.95 

9.19 


%  alcohol 


0 

6.67 
16.02 
22.63 
36.47 


0 

5.50 

6.46 

7.48 

9.24 

41.71 

47.73 

48.27 


0 

2.26 

5.09 

5.96 

8.69 

45.20 

54.19 

68.97 

90.80 


MnSO  4 


36.26 
28.12 
18.75 
12.54 
4.12 


38.6 

32.37 

31.48 

30.51 

28.61 

3.44 

1.58 

1.57 


38.6 

36.31 

33.66 

*33.26 

30.15 

2.49 

0.98 

0.08 

0.01 


*The  solutions  also  sat.  with  respect  to  one 
another. 

(Schreinemakers  and  Deuss.) 


50 


35 


30 


water  layer 


%  alcohol    %  MnSO 


f5.68 

17.69 

t8.70 

fll.85 


18.38 
*9.24 
10.75 
15.09 


f7.60 
*8.69 
10.46 
11.86 
16.18 


34.95 
30.99 
29.20 
24.84 


29.52 
28.61 
26.33 
21.85 


32.40 
30.15 

27.58 
25.75 
20.86 


alcohol  layer 


%  alcohol     %  MnSO 


t53.64 
145.83 
J41.93 
f35.15 


f42.38 
*41.71 
36.89 
30.06 


t50.97 

*45.20 

40.71 

37.54 

29.89 


0.97 
2.19 
3.11 
5.95 


*  3.07 
3.44 
5.19 
9.03 


1.74 
2.49 
3.93 
5.20 
9.64 


(Schreinemakers  and  Deuss.) 
fMetastable  solutions. 
*Solutions  also  sat.  with  respect  to  MnSO< 
H2O. 

Solubility  of  MnSO4+4H2O  in  alcohol +Aq 


g.  H20 


55.86 
52.25 
49.41 
45.34 
42.56 


g.  alcohol 


30.03 
43.59 
47.66 
53.00 
56.24 


MnSO4,  4H2O 


14.11 
4.16 
2.94 
1.66 
1.20 


(Linebarger,  Am.  Ch.  J.  1892,  14.  380.) 

Solubility  of  MnSO4+5H2O  in  alcohol+Ac 
Composition    of    the    solution    sat.    wit 
MnSO4+5H2O. 


10 

15 

17.6 

21 

25 


alcohol  layer 


alcohol       MnSO4 


37.06 
44.56 
47.11 
53.55 
53.09 


5.44 
2.79 
2.22 
1.10 
1.23 


water  layer 


lco°hol         MnSO4 


13.78 

9.25 
8.53 
6.10 
6:81 


25.25 
29.79 
30.88 
35.05 
33.72 


Composition   of   solution    sat.   with   soli 
substance  at  25°. 


%  H20 

%  alcohol 

%  MnSO4 

Solid  phase 

60.7 
*59.47 
*45.68 
42.05 
23.30 

0 
6.81 
53.09 
57.39 
76.70 

39.3 
33.72 
1.23 
0.56 
0.0 

MnSO4+5H20 

11 

a 

ii 

MnSO4+H20 

*The  two  liquids  are  sat.  with  respect  to  o 
another. 


SULPHATE  CUPRIC  OXIDE,  MANGANOUS 


995 


Composition  of  the  two  solutions  sat.  with 
respect  to  one  another  at  25°. 

Manganous  hydrazine  sulphate,  MnH2(SO4)2, 
2N2H4. 
1  pt.  is  sol.  in  60  pts.  H2O  at  18°. 
Stable  in  the  air  at  100°.     (Curtius,  J.  pr. 
1894,  (2)  50.  331.) 

Manganous  nickel  potassium  sulphate, 
MnSO4,    NiSO4,    2K2SO4+12H2O.      Sol. 
in  H2O.    (Vohl,  A.  94.  57.) 

Water  layer 

Alcohol  layer 

%  alcohol 

%  MnS04 

%  alcohol 

%  MnSQ4 

*8.81 

8.48 
15.02 

*33.72 
31.51 
22.61 

*53.09 
49.76 
32.75 

1.23 

1.83 
8.01 

*Also  sat.  with  MnSO4,  5H2O. 

(Schreinemakers  and  Deuss.) 

Insol.  in  absolute  ether  between  5°  and  7°, 
and  no  crystal  H2O  is  removed  thereby. 
Insol.  in  boiling  oil  of  turpentine,  but  1  mol. 
crystal  H2O  is  removed  from  MnSO4+4H2O 
(Brandes,  Pogg.  20.  568.) 

Insol.  in  benzonitrile.  (Naumann,  B.  1914, 
47.  1370.);  ethyl  acetate.  Naumann,  B. 
1910,  43.  314);  acetone.  (Naumann,  B.  1904, 
37.  4329;  Eidmann,  C.C.  1899,  II.  1014.) 

100  g.  sat.  solution  in  glycol  contain  0.5 
g.  MnSO4  (de  Coninck,  Bull.  Ac.  roy.  Belg. 
1905.  359.) 

MnSO4+7H2O  occurs  as  the  min.  Mallar- 
dite. 

Manganomanganic   sulphate,   MnO,    MnO2, 

4S03+9H20. 

Deliquescent.  Decomp.  by  H2O.  Sol.  in 
little  dil.  H2SO4+Aq.  (Fremy,  C.  R.  82. 

475.) 

Manganic  sulphate,  Mn2(SO4)3. 

Extremely  deliquescent.  Sol.  in  H2O  with 
evolution  of  heat,  and  decomposition  into  a 
basic  sulphate.  Behaves  similarly  with 
dilute  acids .  Sol .  in  traces  in  cold  cone .  H2SO 4. 
Insol.  in  cold  cone.  HNO3+Aq.  Sol.  in  cone. 
HCl-f-Aq.  Decomp.  by  absolute  alcohol. 
(Carius,  A.  98.  53.) 

Manganyl  sulphate,  MnO2,  SO3. 

Sol.  in  H2SO4  but  solution  decomp.  if 
below  40-60°  Baume.  Solubility  in  40° 
Baume  acid  =  15%:  55°,  4-5%.  Solution  can 
be  heated  to  60-80°  without  decomp.  (Bad. 
Anilin  u.  Sodafabrik,  C.  C.  1905,  II.  1398.) 

Manganous  hydrogen  sulphate. 

MnSO4  is  sol.  in  20  pts.  boiling  cone.  H2SO4; 
more  sol.  in  boiling  H2SO4+Aq  of  1.6  sp.  gr. 
(Schultz.) 

MnH2(SO4)2,  and+H2O.  Sol.  in  H2O  with 
deoomp.  (Schultz.) 

MnH6(SO4)4.  Sol.  in  H2O  with  decomp. 
(Schultz.) 

Manganic  hydrogen  sulphate,  Mn2H2(SO4)4+ 

8H20. 

Deliquescent.  Decomp.  by  H2O.  Sol.  in 
dil.  H2SO4+Aq.  (Francke,  J.  pr.  (2)  36.  251.) 


Manganous  potassium  sulphate,  K2SO4, 

MnSO4+2H2O. 

+4H2O.  Efflorescent.  (Pierre,  A.  ch.  (3) 
16.  239.) 

2MnSO4,  K2SO4.    (Mallet,    C.  N.  1899, 
80.  301.) 

Manganic  potassium  sulphate,  K2Mn2(S04)4 
+24H2O. 

Decomp.  by  dissolving  in  H2O.  (Mitscher- 
lich.) 

Manganomanganic  potassium  sulphate, 

Mn5(SO4)3,  5K2S04  =  3Mn(SO4)2, 

2MnSO4,  5K2SO4. 

Decomp.  by  much  H2O.  Sol.  in  dil.  or 
cone.  H2SO4.  Insol.  in  alcohol  or  ether. 
(Francke,  J.  pr.  (2)  36.  166.) 

Manganous  potassium  zinc  sulphate,  MnS04, 

2K2SO4,  ZnSO4+12H20. 
Sol.  in  H2O.     (Vohl.) 

Manganous  rubidium  sulphate,  MnSO4, 
Rb2SO4+6H2O. 

Sol.  in  H2O.    (Tutton,  Chem.  Soc.  63.  337.) 

1  1.  H2O  dissolves  357  g.  anhydrous  salt 
at  25°.  (Locke,  Am.  Ch.  J.  1902,  27,  459.) 

+2H2O.  (Wyrouboff,  Bull.  Soc.  Min.  1891, 
14.  242.) 

2MnSO4,  Rb2S04.     (Wyrouboff.) 

Manganic    rubidium    sulphate,    Mn2(S04)«, 

Rb2SO4+24H2O. 

Deliquescent.  (Christensen,  Z.  anorg. 
1901,  27.  333.) 

Manganous  sodium  sulphate,  MnSO4,  Na2SO4. 

+2H2O.  Deliquescent  in  moist  air. 
(Geiger.) 

+4H2O.     Sol.   in    1.2   pts.   boiling   H2O. 

(Geiger.) 

Manganous  sulphate  ammonia,  MnSO 4, 4NH8. 
Decomp.  by  H2O.     (Rose,  Pogg.  20.  148.) 

Manganous  sulphate  cupric  oxide,  MnSO4, 

2CuO+3H2O. 

(Mailhe,    A.  ch.  1902,  (7)  27.  392.) 
MnSO4.    3CuO+zH2O.     (Recoura,  C.  R. 

1901,  132.  1415.) 
MnSO4,  24CuO-fzH2O.      (Recoura.) 


996 


SULPHATE  HYDRAZINE,  MANGANOUS 


Manganous  sulphate  hydrazine,  MnSO4, 
2N2H4. 

Very  unstable. 

Somewhat  sol.  in  NH4OH+Aq.  (Franzen, 
Z.  anorg.  1908,  60.  285.) 

Manganous  sulphate  hydroxylamine,  MnSO4, 

NH2OH+2H2O. 
Insol.  in  H2O.     (Feldt,  B.  1894,  27.  405.) 

Mercurous   sulphate,   basic,   2Hg2O,   S08+ 

H2O. 

Sol.  in  25,000  pts.  H2O  at  20°.  (Gouy,  C. 
R.  1900,  130.  1401.) 

Mercurous  sulphate,  Hg2SO4. 

Sol.  in  500  pts.  cold,  and  300  pts.  hot  H2O. 
(Wackenroder,  A.  41.  319.) 

Solubility  in  H2O  at  18°  =  7.8X10-4  g.  mol. 
per  liter.  (Wilsmore,  Z.  phys.  Ch.  1900,  36. 
305.) 

1  1.  H2O  dissolves  11.71  XHH  g.-mol. 
Hg2SO4  at  25°.  (Drucker,  Z.  anorg.  1901,  28. 
362.) 

Solubility  in  H2O  at  t°. 


t° 

In  100  pts.  of  the  solution 

Hg2SO4  . 

H2S04 

16.5 
33 
50 
75 
91 
100 

0.055 
0.060 
0.065 
0.074 
0.084 
0.092 

0.008 
0.018 
0.037 
0.063 
0.071 
0.071 

(Barre,  A.  ch.  1911,  (8)  24.  203.) 

Solubility  in  H20  at  25°  is  20%  greater 
than  at  18°  and  =  11.71X10-4  g.  mol.  per  1. 
By  addition  of  increasing  amts.  of  H2S04  the 
solubility  is  somewhat,  but  not  regularly, 
decreased,  K2SO4  lowers  solubility  less  than 
H2SO4.  (Drucker,  Z.  anorg.  1901,  28.  362.) 

Easily  sol.  in  dil.  HNOs+Aq,  from  which 
solution  it  is  separated  by  dil.  H2SO4+Aq. 
(Wackenroder,  A.  41.  319.) 

Abundantly  sol.  in  hot,  less  sol.  in  cold  dil. 
H2SO4+Aq.  (Berzelius.) 

Solubility  in  H2SO4+Aq  at  25°. 


H2SO4  normality 

g.-mol.  Hg2SO4  per  litre 

0.0400 
0.1000 
0.2000 

8.31  X  10-4 
8.78  X  10-* 
8.04  X  10-* 

(Drucker,  Z.  anorg.  1901,  28.  362.) 

Partially  .decomp.  by  hot  NH4  salts +Aq. 
(Miahle,  A.  ch.  (3)  6.  179.) 
.     5  times  more  sol.  in  sat.  CdSO4+Aq  than 
in  H2O.    (Hulett,  Phys.  Rev.  1907,  26.  16.) 

Sat.  ZnSO4  or  CdSO4+Aq  attack  much  less 


than  pure  H2O,  yet  the  solubility  of  Hg2SO4 
in  these  solutions  is  greater,  i.  e- ,  0.8  g.  in 
1  1.  ZnSO4+Aq  and  1.1  g.  in  1  1.  CdSO4  + 
Aq  at  20°.  (Gouy,  C.  R.  1900,  130.  1402.) 

Solubility  in  0.2N  K2SO4+Aq  =  9.05X10-4 
g.  mol.  per  1.  at  25°.  (Drucker,  Z.  anorg. 
1901,  28.  362.) 

Solubility  of  Hg2SO4  in  K2SO4+Aq. 


t° 

g.  per  100  g.  sat.  solution 

K2SOi 

Hg2S04 

free  H2SO4 

15 

2.90 
5.70 

8.22 
8.77 
9.44 

0.0475 
0.0703 
0.0912 
0.0994 
0.1080 

0.0080 
0.0093 
0.0098 

o'.oiio 

33 

2.94 
5.68 
8.30 
10.70 
11.90 

0.0677 
0.1015 
0.1364 
0.1724 
0.1902 

0.0250 
0.0350 
0.0441 
0.0438 
0.0420 

75 

3.10 
5.75 
8.50 
13.20 
17.30 

0.1344 
0.2120 
0.2951 
0.4610 
0.6440 

0.1681 
0.2135 
0.2514 
0.2503 
0.2225 

(Barre,  A.  ch.  1911,  (8)  24.  202.) 

About  3  times  as  sol.  in  sat.  ZnSO4+Aq  as 
in  distilled  H2O.     (Wright,  Phil.  Mag.    (5) 
1885,  19.  29.) 

Mercuric  sulphate,  basic,  2HgO,  SO3. 
(Mailhe,  A.  ch.  1902,  (7)  27.  394.) 
3HgO,  SO3.     (Mineral  turpeth.} 

Sol.  in  2000  pts.  cold  and  600  pts.  boiling  H2O. 
(Fourcroy,  A.  ch.  10.  307.) 

Sol.  in  43,478  pts.  H2O  at  16°  when  pptd. 
cold,  and  in  32,258  pts.  at  16°  when  pptd.  at 
100°.  (Cameron,  Z.  anal.  19.  144.) 

SI.  sol.  in  warm  dil.  H2SO4+Aq.    (Rose.) 

Solubility  in  H2O  is  increased  by  addition 
of  H2SO4  up  to  an  acid  content  of  4.3  mol. 
S03  to  93.7  mols.  H2O.  (Hoitsema,  Z.  phys. 
Ch.  1895,  17.  665.) 

Sol.  in  warm  cone.  HC1  or  HBr+Aq. 
(Ditto.) 

Sol.  in  alkali  chlorides  +Aq.    (Miahle.) 

Sol.  in  dil.  HNO8  or  in  HCl+Aq.  More 
easily  sol.  in  the  warm  acids.  (R&y,  Chem. 
Soc.  1897,  71.  1099.) 

3HgO,  2SO3+2H2O.  (Hoitsema,  Z.  phvs. 
Ch.  1895,  17.  659.) 

4HgO,  3SOS.     (Hopkins,  Sill.  Am.  J.  18. 


Mercuric  sulphate,  HgSO4. 

Decomp.  by  H2O  into  3HgO,  SO8,  and  a 
sol.  acid  salt.    Sol.  in  dil.  H2SO4-f  Aq. 
comp.  by  all  acids.    (Berzelius.) 


De- 


SULPHATE, MOLYBDENUM 


997 


Sol.  in  warm  cone.  HC1  or  HBr+Aq;  very 
si.  sol.  in  boiling  cone.  HI+Aq.  (Ditte,  A. 
ch.  (5)  17.  124.) 

Very  si.  sol.  in  hot  cone.  HF.  (Ditte,  A.  ch. 
1879,  (5)  17.  125.) 

Sol.  in  HCN+Aq.    (Mohr.) 

Sol.  with  decomp.  in  NaCl+Aq.    (Miahle.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829. 

Insol.  in  cone,  alcohol. 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329.);  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.);  ethyl  acetate.  (Naumann. 
B.  1910,  43.  314.) 

Insol.  in  benzonitrile.  (Naumann,  B.  1914. 
47.  1370.) 

'  Insol.    in   pyridine.      (Schroeder,    Dissert. 
1901.) 

+H2O.  Decomp.  by  H2O.  (Eisfeldt, 
Pharm.  Centr.  1863.  812.) 

Mercuromercuric  sulphate,  Hg20, 2HgO,  S08. 

Insol.  in  cold  H2O;  not  decomp.  by  boiling 
H2O.  Decomp.  b^HCl+Aq.  (Brooke,  Pogg. 
66.  63.) 

Hg2SO4,  HgSO4.  (Baskerville,  J.  Am. 
Chem.  Soc.  1897,  19.  875.) 

Mercuric  hydrogen  sulphate,  HgH2(SO4)2. 
(Braham,  C.  N.  42.  163.) 

Mercuric  potassium  sulphate,  3HgSO«, 

K2SO4+2H2O. 
Sol.  in  H2O.    (Hirzel,  J.  B.  1860.  332.) 

Mercuric     sulphate     chloride     ammonium 

chloride,  2HgS04,  HgC]2,  2NH4C1. 
Decomp.  with  H2O.     Ether  dissolves  out 
HgCl2.    (Kosmann,  A.  ch.  (3)  27.  238.) 

Mercuric  sulphate  cyanide,  HgSO4,  Hg(CN)2 

+5H20. 

Decomp.  by  cone,  or  warm  acids.  (Rupp, 
Arch.  Pharm.  1912,  260.  280.) 

Mercuric  sulphate  hydrazine,  HgS04,  N2H4. 
Ppt.     (Hofmann  and  Marburg,  A.  1899, 
306.  216.) 

Mercuric    sulphate    hydrobromide,    HgSO4, 
2HBr. 

Sol.  in  H2O  without  separation  of  basic  sul- 
phate. (Ditte,  A.  ch.  (5)  17.  122.) 

3HgO,  SO3,  6HBr.    Sol.  in  H2O.     (Ditte.) 

Mercuric    sulphate    hydrochloride,    HgSO4, 
HC1. 

Not  attacked  by  HC1.  SI.  sol.  in  HNO3. 
(Baskerville,  J.  Am.  Chem.  Soc.  1901,  23. 
895.) 

HgSO*,  2HC1.  Sol.  in  H2O  without  sep- 
aration of  a  basic  salt.  Very  sol.  in  warm 
H2SO4,  solidifying  on  cooling  if  very  cone., 
or  crystallising  if  dil.  (Ditte.) 


Very  deliquescent. 

Very  sol.  in  H2O.  (Baskerville,  J.  Am. 
Chem.  Soc.  1901,  23.  895.) 

+H2O.  (Baskerville,  J.  Am.  Chem.  Soc. 
1901,  23.  895.) 

3HgO,  SO3,  6HC1.    Sol.  in  H2O.     (Ditte.) 

Mercuric    sulphate   hydroxylamine.   HgSO4, 

2NH2OH+H20. 

Decomp.  by  cold  H2O.  (Adams,  Am.  Ch. 
J.  1902,  28.  209.) 

Mercuric  sulphate  iodate  iodide,   6(3HgO, 

2S08),  6HgI2,  Hg(I03)2. 
Decomp.  by  H2O  and  acids.     (Bruckner, 
M.  1907,  28.  961.) 

Mercuric  sulphate  iodide,  basic,  3HgO,  2SO,, 
HgI2. 

3(3HgO,  2SO3),  2HgI2  +  10H2O. 

2(3HgO,  2SO3),  HgI2  +  10H2O.  Very  sol. 
in  hot  cone.  HNOs. 

3HgO,  2S03,  HgS04,  HgI2  +  10H20. 
(Ditte,  C.  R.  1905,  140.  1167.) 

Mercuric  sulphate  iodide,  HgS04,  HgI2. 

Decomp.  by  H2O,  not  by  alcohol  or  ether. 
(Riegel,  J.  B.  pr.  Pharm.  11.  396.) 

3HgSO4,  HgI2.  Decomp.  by  cold  or  hot 
H2O.  Sol.  in  H2SO4+Aq.  (Ditte,  C.  R. 
1905,  140.  1165.) 

4HgSO4,  HgI2  +  15H2O,  and  +  18H2O.  De- 
comp. by  cold  or  hot  H2O. 

Sol.  in  H2SO4.    (Ditte.) 

Mercuric  sulphate  phosphide. 

See  Dimercuriphosphonium  mercuric  sul- 
phate. 

Mercuric  sulphate  sulphide,  basic,  2HgO, 
S03,  HgS. 

Somewhat  sol.  in  HC1,  H2SO4  and  HNO3. 
(Jacobson,  Pogg.  1846,  68.  412. 

4HgO,  3SO3,  2HgS+4H2O.  SI.  sol.  in 
H2SO4.  (Estrup,  Z.  anorg.  1909,  62.  169.) 

Mercuric  sulphate  sulphide,  2HgSO4,  HgS. 
SI.  sol.  in  hot  HC1,  H2SO4,  or  HNO3+Aq. 

Easily  sol.   in  hot  aqua  regia.      (Jacobson, 

Pogg'  68.  410.) 

2HgSO4,  HgS.  (Palm,  C.  C.  1863.  122.) 
HgSO4,  2HgS.  (Barfoed,  J.  B.  1864.  282.) 
Sol.  in  aqua  regia.  (Deniges,  Bull.  Soc. 

1915,  (4)  17.  355.) 
HgSO4,  3HgS.    Insol.  in  H2O.    Easily  sol. 

in  aqua  regia;  decomp.  by  HNO3  into — 
3HgSO4,  HgS.     Insol.  in  all  acids  except 

aqua  regia.     (Spring,  A.  199.  116.) 

Molybdenum  sesgwisulphate  (?). 

Basic.    Insol.  in  H2O. 

Neutral.  Decomp.  by  H2O  into  acid  and 
basic  salts. 

Acid.    Sol.  in  H2O.    (Berzelius.) 


SULPHATE,  MOLYBDENUM 


Molybdenum  cfo'sulphate  (?). 
Sol.  in  H2O. 

Molybdenum  sulphate,  Mo2O5,  2SO3. 

Very  slowly  sol.  in  cold,  more  quickly  sol. 
in  hot  H2O.  (Bailhache,  C.  R.  1901, 132.  476.) 

7MoO3,  2MoO2,  7SO3+Aq.  (Pechard,  C. 
R.  1901,  132.  630. 

Molybdic  sulphate,  MoO3,  SO8. 

Deliquescent.  Sol.  in  H2O.  (Schultz- 
SeUack,  B.  4.  14.) 

MoO3,  3SO3+2H2O.  Deliquescent.  Par- 
tially sol.  in  H2O.  (Anderson,  Berz.  J.  B.  22. 
161.) 

Does  not  exist.    (Schultz-Sellack.) 

Molybdenum  sulphate  ammonia, 

5NH3,  MoO2SO8,  7MoO3+8H2O. 

3NH3,  MoO2SO3,  7MoO3  +  10H2O. 
Both  very  sol.  in  water  but  less  sol.  in  H2O 
containing  ammonium  salts.    (Pechard,  C.  R. 
1901,  132.  630.) 

Neodymium  sulphate,  basic,  Nd2O3,  SO3. 

Insol.  in  H2O. 

Nearly  insol.  in  dil.  acids.  (Wohler,  B. 
1913,  46.  1730.) 

Insol.  in  H2O.  (Matignon,  C.  R  .1902, 
134.  658.) 

Neodymium  sulphate,  Nd2(SO4)3+8H2O. 
Solubility  in  100  pts.  H2O  at  t°. 


t° 

pts.  Nd2(SO4)s 

0 

9.50 

16 

7.05 

30 

5.04 

50 

3.72 

80 

2.70 

100 

2.21 

(Muthmann  and  Rolig,  B.  1898,  31.  1728.) 

Neodymium  hydrogen  sulphate,  Nd(S04H)3. 
(Brauner,  Z.  anorg.  1904,  38.  331.) 

Neodymium  potassium  sulphate. 

Cryst.  modification  more  sol.  in  cold  than 
in  hot  H2O.  (Boudouard,  C.  R.  1898,  126. 
901.) 


(Berzelius.) 
(Athanasesco,  C.  R. 


Nickel  sulphate,  basic. 

Very  si.  sol.  in  H2O. 

6NiO,  5SO3+4H2O. 
103.  271.) 

7NiO,   7H2O,   SO3+3H2O.     Nearly  insol. 
in  H2O.    (Habermann,  M.  5.  432.) 

5NiO,  SO3;  5NiO,  2SO3;  and  5NiO,    3SO3. 
(Pickering,  Chem.  Soc.  1907,  91.  1985.) 

6NiO,  SO3.  (Stromholm.  C.C.  1906, 1. 1222.) 


Nickel  sulphate,  NiSO4. 

100  pts.  H2O  dissolve  pts.  N1SO4  at  t°: 

2°          16°         20°         23°         31° 
30.4       37.4       39.7        41         45.3  pts.  NiSCh, 

41°         50°        53°          60°         70° 
49.1         52         54.4       57.2  "    61.9  pts.  NiSO4. 
(Tobler,  A.  95.  193.) 

100  pts.  of  sat.  solution  contain:  at  11-14°,  28.84; 
at  18-20°,  30.77  pts.  anhydrous  salt.  (v.  Hauer,  W. 
A.  B.  53,  2.  221.) 

100  pts.  H2O  at  112.5°  dissolve  185.71  pts.  NiSCU. 
(Griffiths.) 

NiSO4+7H2O  is  sol.  in  3  pts.  H2O  at  12.5°.     (Tup- 

PU100  pts.  H2O  at  15.5°    dissolve    75.6  pts.  NiSC>4  + 
7H20. 

Sat.  NiSO4-f-Aq  contains  at: 
—3°    +2°      5°       11°      17°     54° 
21.7    22.7    23.1    25.2    26.6    33.6%  NiS04. 

68°    74°    92°    97°  110°  117°  119° 
38.2  38.7  42.4  44.2  46.5  48.8  49.4%  NiSO4. 
(fitard,  A.  ch.  1894,  (7)  2.  552.) 

See  also  below  under  hydrated  salts. 
Sp.  gr.  of  NiSO4'+Aq  containing  g.  NiSO4+ 
7H2O  in  1000  g.  H2O  at  23.5°. 

140.5  g.  ( =  Y*  mol.)  281      421.5     562 
1.073  1.136     1.190     1.238 


602.5 
1.280 


843 
1.317 


983.5 
1.349 


1124 
1.378 


Containing  NiSO4  (anhydrous) : 
77.5g.(  =  i/2mol.)  155  232.5  310  387.5  465 
1.079  1.153  1.224  1.292  1.358  1.421 

(Gerlach,  Z.  anal.  28.  468.) 


Sp.  gr.  of  NiSO4+Aq  at  0°.    S  =  pts.  NiSO4 
in  100  pts.  solution;  Si  =  mols.  NiSO4  in 
100  mols.  solution. 

s 

Si 

Sp.  gr. 

4.2930 
3.9591 
3.2845 
2.5043 
1.6131 
0.8327 

0.581 
0.476 
0.392 
0.297 
0.189 
0.097 

.0522 
.0431 
.0357 
.0271 
.0173 
.0089 

(Charpy,  A.  ch.  (6)  29.  26.) 

Sp.  gr.  of  NiSO4+Aq  at  room  temp,  con- 
taining: 

10.62        18.19        25.35%  NiS04. 
1.0925      1.1977      1.3137 
(Wagner,  W.  Ann.  1883,  18.  272.) 

Sp.  gr.  of  NiSO4+Aq  at  25°. 


Concentration  of  NiSO4 
+Aq 

Sp.gr 

1-normal 

Vi-     " 

l/4_    « 
l/g-    " 

1.0773 
1.0391 
1.0198 
1.0017 

(Wagner,  Z.  phys.  Ch.  1890,  6.  39.) 

SULPHATE,  NICKEL 


999 


For  solubility  of  NiSO4+Na2SO4  in  H2O, 
see  under  NiSO4+7H2O  and  NiNa2(SO4)2. 
100  pts.  sat.  NiSO4+ZnSO4+Aq  at  18-20° 
contain  35.45  pts.  of  the  two  salts,    (v.  Hauer.) 
Insol.  in  liquid  NH3.      (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 
HC2H3O2  precipitates  it  completely  from 
aqueous  solution.     (Persoz.) 
100  pts.  absolute  methvl  alcohol  dissolve 
0.5  pt.  NiSO4  at  18°.     (de  Bruyn,  Z.  phys. 
Ch.  10.  783.) 

Solubility  of  NiSO4,  3CH4O+3H2O  in  methyl 
.  alcohol  at  14°. 

P  =  %  anhydrous  NiS04  in  the  sat.  solu- 
tions. 

+6H2O.       Two    modifications.      a-blue, 
tetragonal;  /3-green,  monoclinic. 

Solubility  of  a-  NiSO4,  6H2O  in  H20  at  t°. 

Salt  used 

t° 

g.  N1SO4 
in  100 
g.  H2O 

Salt  remaining 

NiS04+6H20  (blue) 

NiSO4+7H2O 

NiSO4+6H20 
NiSO4+7H2O 
NiS04+6H2O  (blue) 

32.3 

33.0 
34.0 
35.6 
44.7 
44.7 
50.0 
51.0 
52.0 
53.0 

43.57 

43.35 
43.84 
43.79 
48.05 
47.97 
50.15 
50.66 
52.34 
52.34 

NiSO4  +  6H2O 
(blue) 

(Steele  and  Johnson.) 
Solubility  of  /3-  NiSO4,  6H2O  in  H2O  at  t°. 

Alcohol 

1% 

by  wt. 

P 

In  1000  mol.  of  the  solution 

Mol. 
NiSO4 

Mol. 
CH40 

Mol. 
H2O 

Salt  used 

t° 

g.  NiS04 
per  100 
g.H20 

Salt  remaining 

100 
97.5 
95 
92.5 
90 
89 
88 
87 
86 
85 

3.72 
0.77 
0.455 
0.50 
0.70 
1.01 
1.25 
1.48 
1.73 
1.93 

7.75 
1.65 
0.96 
1.0 
1.6 
2.0 
2.4 
2.9 
3.2 
3.6 

969 
950 
908 
871 
830 
814 
800 
781 
767 
755 

23.2 

48.5 
91 
128 
168 
184 
198 
216 
230 
241 

NiSO4+6H2O(blue) 

NiSO4+6H2O(blue) 
NiS04+7H20 
NiSO4+6H2O(blue) 
NiS04  +7H20 
NiS04+7H20 

NiS04+6H20(blue) 
NiSO4+6H2O(blue) 
NiS04+7H20 
N1SO4  +7H2O 

54.5 
157.0 

jeo.o 

69.0 
70.0 
73.0 

80.0 

89.0 
99.0 

52.50 

53.40 

54.84 

58.38 
59.44 
60.72 

63.17 
67.90 
76.71 

NiSO4+6H2O 
(green) 

(de  Bruyn,  R.  t.  c.  1903,  22.  418.) 


This  salt  is  more  sol.  in  ethyl  alcohol  than 
in  methyl  alcohol. 

See  also  under  hydra  ted  salts. 

For  solubility  of  NiSO4  in  ethyl  alcohol, 
see  under  hydrated  salts. 

100  g.  sat.  solution  in  glycol  contain  9.7  g. 
NiSO4  at  ord  temp,  (de  Coninck,  Bull.  Ac. 
Roy.  Belg.  1906.  359.) 

Insol.  in  methyl  acetate.  (Naumann, 
B.  1909,  42.  3790);  ethyl  acetate,  (Naumann, 
B.  1904,  37,  3602.) 

Very  si.  sol.  in  acetone.  (Krug  and 
M'Elroy.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329;  Eidmann,  C.  C.  1899,  II.  1014). 

+H2O.  Very  si.  sol.  in  abs.  methyl  al- 
cohol. After  standing  in  contact  with  it  for 
8-9  months,  the  solution  contains  1.34% 
NiSO4.  (de  Bruyn.  R.  t.  c.  1903,  22.  414.) 

+2H2O.  Cryst.  from  sat.  NiSO4-f  Aq  at 
131°.  (Steele  and  Johnson.) 

+4H2O.     Solubility  in  methyl  alcohol + 
Aq  at  10°.    Time  =  24  hrs.    P=%  anhydrous 
salt  in  the  sat.  solutions. 
Alcohol  of     100%   80%   50%    20%    water 
P  7.38     0.66     1.43     14.8      25.1 

(de  Bruyn,  R.  t..c.  1903,  22.  414.) 


(Steele  and  Johnson,  Chem.  Soc.  1904,  86. 
118.) 

Tr.  point  from  a-  to  /3-  salt  =  53.3°.  (Steele 
and  Johnson.) 

100  pts.  absolute  methyl  alcohol  dissolve 
31.6  pts,  NiS04+6H2Oat  17°;  100  pts.  93.5% 
methyl  alcohol  dissolve  7.8  pts.  NiSO4+ 
6H2O  at  18°;  100  pts.  50%  methyl  alcohol 
dissolve  1.9  pts.  NiSO4+6H2O  at  18°.  (de 
Bruyn,  Z.  phys.  Ch.  10.  786.) 

a-Salt.     Solubility    in    methyl    alcohol +Aq 
at  14°.     Time  =  5  to  6  hrs. 


Alcohol 
%  by  wt. 

N§04 

In  1000  mol.  of  the  solution 

Mol. 
NiSO4 

Mol. 
CH4O 

Mol. 
HaO 

100 

12.4 

26 

794 

180 

97.5 

10.6 

22.3 

808 

170 

95 

6.5 

14 

817 

169 

92.5 

3.06 

5.9 

838 

156 

90 

1.18 

2.3 

821 

177 

85 

0.315 

0.57 

757 

242 

80 

0.25 

0.4 

688 

312 

60 

0.46 

0.8 

453 

546 

40 

2.43 

3.5 

265 

732 

20 

14.7 

21 

105 

874 

0  (water) 

26.0 

39 

0 

961 

(de  Bruyn,  R.  t.  c.  1903,  22.  412.) 

1000                                               SULPHATE,  NICKEL 

/3-salt.     Solubility  in  methyl  alcohol  +Aq  at 

Solubility  in  100  pts.  H2O  at  t°.  —  Continued. 

14°.     Time-24hrs. 

Pts 

Pts. 

Pts 

Alcohol 

O7 

In  1000  mol.  of  the  solution 

t 

NIS04 

t 

NiSO4 

t° 

NiS04 

%  by  wt. 

% 

NiSCU 

Mol. 

Mol. 

Mol. 

99 

83.1 

103 

85.6 

107 

88.1 

NiS04 

CHiO 

H20 

100 

83.7 

104 

86.2 

108 

88.7 

100 

15.7 

33.8 

763 

203 

101 
102 

84.3 
84.9 

105 
106 

86.8 
87.5 

108.4 

88.7 

97.5 

12.4 

26 

781 

193 

95 
92.5 
90 
89 

10.0 
5.61 
2.35 
1.79 

20.3 
11.1 
4.5 

784 
800 
810 

196 
189 
185 

(Mulder,  calculated  from  his  own  and  Tob- 
ler's  determinations,  Scheik.  Verhandel.  1864. 

70.) 

88 

1.29 

87 

0  97 

t 

86 

0^73^ 

Solubility  in  H2O  at  t°. 

OK 

OA1 

10 

*7K  K 

C\A    A 

oo 
80 
60 

.  Dl 

0.41* 
0.75 

.0 

)     0.7 
1.3 

/GO 

682 
453 

J44 

•317 
546 

Salt  used 

t° 

g.  NiSO 
in  100 
gH20 

Salt  remaining 

40 

3  11 

4  0 

264 

700 

20 

14!  1 

2LO 

^/l_r± 

105 

i  O—  ' 

874 

NiSO 

4+7H2O 

—  5 

25.74 

NiSO 

4+7H20 

0  (water) 

27.2 

40.0 

0 

960 

tt 

0 

27.22 

O1       Ct  C 

(de  Bruyn.) 

tt 

15 

ol  .00 

34.19 

(( 

22.6 

37.90 

_j_7jj2O 

tt 

22.8 

38.88 

Solubility  in  100  pts.  H2O  at  t°,  using 

NiSO4+7H2O. 

NiSO 
NiSO 

tt 

4+6H2O 
4+7H20 

30.0 
30.0 
32.3 

42.46 
42.47 
44.02 

Pts 

Pts' 

Pts 

33.0 

45.74 

t° 

NiS04 

t° 

N1SO4 

t° 

NiS04 

u 

34.0 

45.5 

tt 

0 

29.3 

33 

45.5 

66 

63.6 

(Steele  and  Johnson, 

Chem.  Soc.  1904,  85. 

1 

29.7 

34 

46.0 

67 

64.1 

116.) 

2 

30.1 

35 

46.5 

68 

64.7 

3 

30.5 

36 

47.0 

69 

65.3 

4 
5 
6 
7 
8 
9 
10 

31.0 
31.5 
32.0 
32.5 
33.0 
33.5 
34.0 

37 
38 
39 
40 
41 
42 
43 

47.5 
48.0 
48.5 
49.0 
49.6 
50.1 
50.6 

70 
71 
73 

72 
74 
75 
76 

65.9 
66.5 
67.0 
67.6 

68.2 
68.8 
69.3 

M.-pt.   of  NiSO4+7H2O  =  98-100°.      (Til- 
den,  Chem.  Soc.  45.  409.) 
Tr.  point  from  a-6H2O  salt  to  7H20  salt  = 
31.5°.    (Steele  and  Johnson.) 
Exists  also  in  an  unstable,  more  soluble 
modification.      (Fedorow,     C.   C.   1903,  II. 

f\f   \ 

11 

34.5 

44 

51.2 

77 

69.9 

95.) 

12 

35.0 

45 

51.7 

78 

70.5 

13 
14 

35.5 
36.0 

46 

47 

52.3 

52.8 

79 
80 

71.1 

71.7 

Solubility    of    NiSO4 

.7H2O+Na2SO4.10H2O 

15 

1  C* 

36.5 

O^7     f\ 

48 

53.4 

81 

72.3 

in  100  g. 

H2O  at  t°. 

16 
17 

37.0 
37.5 

49 
50 

53.9 
54.5 

82 
83 

72.9 
73.5 

.t° 

grams  N1SO4 

grams  NazSCh 

18 
19 
20 
21 

38.0 
38.5 
39.0 
39.5 

51 
52 
53 
54 

55.0 
55.6 
56.1 
56.7 

84 
85 
86 

87 

74.1 
74.6 
75.2 

75.8 

0 
5 
10 

22 
25 

28 

.46 

.28 
.26 

10.09 
15.245 
20.64 

22 
23 
24 

40.0 
40.5 
41.0 

55 
56 
57 

57.3 
57.9 
58.4 

88 
89 
90 

76.4 
77.0 
77.6 

(Koppel,  Z.  phys.  Ch.  1905,  52.  401.) 

See  also  under  NiNa2(SO4)4. 

25 

41.5 

58 

59.0 

91 

78.2 

26 
27 
28 
29 
30 
31 
32 

42.0 
42.5 
43.0 
43.5 
44.0 
44.5 
45.0 

59 
60 
61 
62 
63 
64 
65 

59.6 
60.2 
60.7 
61.3 
61.9 
62.4 
63.0 

92 
93 
94 
95 
96 
97 
98 

78.8 
79.4 
80.1 
80.7 
81.3 
81.9 
82.5 

100  pts.  absolute  methyl  alcohol  dissolve  46 
pts.  NiSO4+7H2O  at  17°;  100  pts.  absolute 
methyl   alcohol   dissolve   24.7   pts.    NiSO4+ 
7H2O  at  4°;  100  pts.  93.5%  methyl  alcohol  dis- 
solve 10.1  pts.  NiSO4+7H2O  at  4°;  100  pts. 
50%  methyl  alcohol  dissolve  2  pts.  NiSO4+ 
7H2O  at  4°.    (de  Bruyn,  Z.  phys.  Ch.  10.  786.) 

SULPHATE,  NICKEL  ZINC 


1001 


Solubility    in    methyl    alcohol  +Aq    at    14' 
Time,  5  to  6  hrs. 


A  1^_U      1 

In  1000  mol.  of  solution 

Alcohol 
%  by  wt. 

NiS()4 

Mol. 

Mol. 

Mol. 

NiSO4 

CH4O 

H20 

100 

16.8 

35.7 

714 

250 

97.5 

13.9 

29 

734 

237 

95 

11.6 

23.6 

742 

234.5 

92.5 

8.12 

16.2 

760 

224 

90 

5.78 

11.2 

758 

231 

85 

1.52 

3 

744 

253 

84 

1.06 

. 

. 

.  .  . 

83 

0.985 

. 

82 

0.83 

81 

0.665 

80 

0.653 

1^2 

687 

312 

60 

0.805 

1.3 

453 

546 

45 

1.73 

40 

2.78 

4 

264 

732' 

35 

4.55 

30 

6.33 

20 

13.7 

20" 

105 

875' 

0  (water) 

26.4 

39.5 

0 

960.5 

(de  Bruyn,  B.  t.  c.  1903,  22.  411.) 

* 

100  g.  absolute  ethyl  alcohol  dissolve  1.3 
g.  NiSO4+7H2O  at  4°,  and  2.2  g.  at  17°.  (de 
Bruyn,  Z.  phys.  Ch.  10.  786.) 

Min.  Moreno  site. 

Nickel  hydrazine  sulphate,  NiH2(SO4)2, 

2N2H4. 

1  pt.  is  sol.  in  275.5  pts.  H2O  at  18°.  SI. 
sol.  in  hot  H2O.  Sol.  in  HNO3  with  decomp.; 
insol.  in  HC1.  Sol.  in  NH4OH+Aq.  (Cur- 
tius,  J.  pr.  1894,  (2)  60.  331.) 

Nickel  potassium  sulphate,  NiSO4,  K2SO4+ 
6H2O. 

Sol.  in  8-9  pts.  H2O.    (Tupputi.) 

100  pts.  H20  dissolve  at: 
0°    10°    14°     20°     30° 
5.3  8.9    10.5   13.8    18.6  pts.  anhydrous  salt, 

36°    49°    55°    60°    75° 
20.4  27.7  32.4  35.4  45.6  pts.  anhydrous  salt. 
(Tobler,  A.  96.  193.) 

Saturated  solution  contains  at: 
20°      40°      60°      80° 
8.7     12.3     17.6    22.0%  anhydrous  salt, 
(v.  Hauer,  J.  pr.  74.  433.) 


Nickel  rubidium  sulphate,  NiSO4,  Rb2SO4-h 
6H20. 
Sol.  in  H2O.    (Tutton,  Chem.  Soc.  63.  337.) 
1    1.    H2O    dissolves    59.8    g.    anhydrous 
salt  at  25°.    (Locke,  Am.  Ch.  J.  1902,  27.  459.) 

Nickel  sodium  sulphate,  NiNa2(SO4)2+4H20. 

Solubility  of  NiNa2(SO4)2.4H2O  in  100  g.  H2O 
at  t°. 

t° 

grams  NiSO4 

grams  Na2SC>4 

20 
25 
30 
35 

.       40 

29.31 
27.33 
24.64 
23.66 

21.88 

26.87 

25.33 
22.58 
21.67 
20.65 

(Koppel,  Z.  phys.  Ch.  1905,  52.  401.) 

Solubility      of      NiNa2  (SO4)  2.4H2O  +  NiSO4  . 
7H2O  in  100  g.  H2O  at  t°. 

•  o          grams 
N1SO4 

grams           ,0 
NaSO4 

grams        grams 
N1SO4       Na2SO4 

18.5     30.70 
20        31.59 
25        33.11 

25.805       30 
25.355       35 
23.07         40 

34.98     19.825 
36.01     16.435 
37.935    14.295 

(Koppel.) 

Solubility    of     NiNa2(SO4)2.4H2O+Na2SO4. 
10H2O  in  100  g.  H2O  at  t°. 

t°                     grams  N1SO4 

grams  NaSO4 

18.5                   26.14 
20                      24.07 
25                       18.81 
30                        9.87 

29.455 
31.365 
37.13 
44.25 

(Koppel.) 

Solubility  of  NiNa2(SO4)2.4H2O+Na2SO4 
(anhydrous)  in  100  g.  H2O  at  t°. 

t° 

grams  N1SO4 

grams  Na2SO4 

35 
40 

7.13 
7.245 

49.595 
49.03 

(Koppel.) 

Nickel  thallium  sulphate,  NiSO<,  T12SO4+ 
6H2O. 

Easily  sol.  in  H2O.  Can  be  recryst.  from 
little  H2O  without  decomp.  (Werther,  J.  pr. 
92.  132.) 

1  1.  H2O  dissolves  46.1  g.  anhydrous  salt 
at  25°.  (Locke,  Am.  Ch.  J.  1902,  27,  459.) 


1    1.    H2O    dissolves    68.8    g.    anhydrous 
salt  at  25°.    (Locke,  Am.  Ch.  J.  1902,  27. 459.) 


Nickel    potassium    zinc    sulphate, 

2K2SO4,  ZnSO4+12H2O. 
Sol.  in  H2O.    (Vohl,  A.  94.  51.) 


Nickel  zinc  sulphate,  NiSO4,  ZnS04+13H20. 

Sol.  in  3-4  pts.  cold  H2O.    Insol.  in  alcohol. 
(Tupputi,  1811.) 
NiSO4,       Completely  sol.  in  NH4OH+Aq. 

2NiSO4,  2ZnSO4,  H2SO4.     (Etard,  C.  R. 
87.  602.) 


1002 


SULPHATE  AMMONIA,  NICKEL 


Nickel  sulphate  ammonia,  NiS04,  6NH8. 

Sol.  in  H2O  with  separation  of  hydroxide. 
(Rose,  Pogg.  20.  151.) 

NiSO4,    5NH3+3^H2O.      Deliquescent. 
(Andre,  C.  R.  106.  936.) 

NiSO4,  4NH3+2H2O.  Easily  sol.  in  H2O. 
Can  be  recrystallized  out  of  little  H2O.  In- 
sol.  even  in  dil.  alcohol.  (Erdmann.) 

Nickel  sulphate  cupric  oxide,  NiS04,  2CuO+ 
6H2O. 

(Mailhe,  Bull.  Soc.  1902,  (3)  27.  172.) 

2NiSO4,  3CuO  +  10H2O,  and  +12H2O. 
(Mailhe.) 

5NiSO4,  16CuO+zH2O.  (Recoura,  C.  R. 
1901,  132.  1415.) 

NiSO4,  20CuO+zH2O.     (Recoura.) 

Nickel  sulphate,  hydrazine,  NiSO4,  3N2H4. 
Ppt.    (Curtius,  J.  pr.  1894,  (2)  50.  343.) 

Nickel  sulphate  hydroxylamine,  NiSO4, 
6NH2OH. 

Decomp.  by  H2O.  (Uhlenhut,  A.  1899, 307. 
334.) 

Nitrosyl  sulphate,  H(NO)SO4. 
See  Nitrosulphonic  acid. 

Osmious  sulphate. 
Easily  sol.  in  H2O  and  alcohol. 

Osmic  sulphate. 

Sol.  in  H2O.     (Berzelius.) 

Palladous  sulphate,  basic,  PdS04,  7PdO  + 

6H2O,  and  10H2O. 

Insol.  in  H2O.  Easily  sol.  in  HCl+Aq. 
(Kane.) 

Palladous  sulphate,  PdS04+2H2O. 

Deliquescent  in  moist  air;  very  sol.  in  H2O, 
but  decpmp.  by  much  H2O,  with  separation 
of  a  basic  salt.  (Kane.) 

Phosphoryl  sulphate,  (PO)2(S04)»  (?). 

Possible  composition  of  Weber's  (B.  20. 
86)  P2O6,  3SO3  (?). 

3P2O4,  2SO«.  Immediately  decomp.  by 
H2O.  (Adie,  G.  N.  1891,  63.  102.) 

Platinic  sulphate,  Pt(SO4)2. 

Deliquescent.  Sol.  in  H2O,  alcohol,  or 
ether;  also  in  H3PO4,  HC1,  and  HNO3+Aq. 
(Berzelius.) 

H2PtO2SO4.  Sol.inH20.  (Blondel,  A.  ch. 
1905,  (8)  6.  109.) 

PtO2,  SO3+4H2O.  Ppt.  Decomp.  by  H20. 
Sol.  in  H2SO4. 

PtSO4(OH)2,    4Pt(OH)4+3H2O.      Ppt. 
(Prost,  Bull.  Soc.  (2)  46.  156.) 

Pt8SO4Oi3  +  16H2O.    As  above.     (Prost.) 


Platinum  hydroxylamine  sulphate, 
Pt(NH2OH)4SO4. 

Only  si.  sol.  in  H2O;  sol.  in  dil  H2SO4+Aq. 
(Uhlenhut,  A.  1900,  311.  123.) 

Platinic  potassium  sulphate,  basic. 

Insol.  in  boiling  H2O,  HNO3,  H2SO4, 
HsPO^,  HC2H3O2,  or  NH4OH+Aq.  Easily 
sol.  in  boiling  HCl+Aq.  SI.  decomp.  by 
aqua  regia.  (E.  Davy.) 

Ptio(SO4)2Oio,  3K2SO4+34H2O.  Insol.  in 
H2O.  (Prost,  Bull.  Soc.  (2)  46.  156.) 

Pti8(SO4)O22,  5K2SO4+34H2O.  As  above. 
(Prost.) 

Platinum  rubidium  sulphate,  Pt6Rb6(SO4)4  + 

17H2O. 
Sol.  in  H2O.    (Prost,  Bull.  Soc.  (2)  46.  156.) 

Platinum  sulphate  sulphocarbamide,  PtSO4, 

4CS(NH2)2. 

Insol.  in  H2O.  Sol.  in  cone.  H2SO4  without 
decomp.  (Kurnakow.  J.  pr.  1894,  (2)  50, 
489.) 

Potassium  sulphate,  K2S04. 

Not  hygroscopic  in  the  ordinary  sense  of  the 
word.  100  pts.  K2SO4  over  H2O  at  14-20° 
absorb  58  pts.  H20  in  22  days,  and  finally  de- 
liquesce completely.  (Mulder.) 

12  pts.  K2SO4  mixed  with  100  pts.  H2O 
lower  the  temp.  3.3°.  (Riidorff,  B.  2.  68.) 

100  pts.  H2O  dissolve  with  absorption  of 
heat  at  0°: 

8.36  pts.  K2SO4.    (Gay-Lussac.) 

8.46         "  (Mulder.) 

8.5  "  (Gerardin.) 

7.31         "  (Moller,  Pogg.  117.  386.) 

7.3-7.9  "  (Nordenskiold,  Pogg. 

136.314.) 

100  pts.  H2O  at  0°  dissolve  8.36  pts.  K2SC>4;  at  12.72°, 
10.57  pts.;  at  49.08°,  16.91  pts.;  at  63.90°,  19.29  pts.; 
at  101.50°,  26.33  pts.  (Gay  Lussac,  A.  ch.  (2)  11.  311.) 


Solubility  in  100  pts.  H2O  at  t°. 


t° 

Pts. 
K2S04 

t° 

Pts. 
K2S04 

0 
15.65 
28.1 

7.8 
10.3 
12.8      - 

47.0 
70.2 
98.0 

16.0 
20.3 
23.9 

(Nordenskiold,  Pogg.  136.  341.) 

100  pts.  sat.  K2SO4  at  101.7°  contain  17.5  pts.  K2SO4, 
or  100  pts.  H2O  at  101.25°  dissolve  21.212  pts.  K2SO4. 
(Griffiths.) 

100  pts.  H2O  at  102.8°  dissolve  29  pts.  K2SO4  (Penny) ; 
at  15°,  7.3-6.25  pts.  (Ure's  Diet.);  at  100°,  20  pts. 
(Ure's  Diet.);  at  100°,  24.2  pts.  (Wenzel). 

Sol.  in  9.081  pts.  H2O  at  15°  (Gerlach) ;  in  16  pts.  at 
15°,  and  5  pts.  at  100°  (Bergmann) ;  in  18  pts.  cold,  and 
5  pts.  boiling  H2O  (Fourcroy);  in  15  pts.  cold,  and  5  pts. 
boiling  H2O  (Reid);  in  12  pts.  H2O  at  0°,  and  4  pts. 
boiling  H2O  (M.  R.  and  P.);  in  12  pts.  H2O  at  18.75° 
(Abl) 

K2SO4  sat.  at  15°  has  sp.  gr.  =1.0774,  and  contains 
10.055  pts.  K2SO4  ip  100  pts.  H2O.  (Michel  and 
Krafft,  A.  ch.  (3)  41.  478.) 

100  pts.  H2O  dissolve  9.26  pts.  K2SO4  at 
15.6°,  and  sat.  solution  has  sp.  gr.  =  1.177. 
(Page  and  Keightley,  Cheir.  Soc.  (2)  10.  566.) 


SULPHATE,  POTASSIUM 


1003 


Solubility  in  100  pts.  H2O  at  t°. 

100  ccm.  H2O  dissolve  12.04  g.  K2SO4  at 
25°.     (Trevor,  Z.  phys.  Ch.  7.  468.) 
Sat.  K2S04+Aq  contains  at: 
21°        23°        60°        99°        130° 
10.1       10.3       14.5       19.1       21.1%K2SO4, 

130°      152°      175°      195°      220° 
21.3      22.8      24.5       23.8       24.6%  K2S04. 
(fitard,  A.  ch.  1894,  (7)  2.  549.) 

Solubility  of  K2SO4  in  H2O  at  t°. 
G.  K2SO4  per  100  g.  H2O 

t° 

Pts. 
K2S04 

t° 

Pts. 
K2S04 

t° 

Pts. 
KiS04 

0 
1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
34 

8.5 
8.6 
8.7 
8.8 
9.0 
9.1 
9.2 
9.3 
9.4 
9.5 
9.7 
9.8 
9.9 
10.0 
10.2 
10.3 
10.4 
10.5 
10.7 
10.8 
10.9 
11.1 
11.2 
11.3 
11.5 
11.6 
11.7 
11.9 
12.0 
12.2 
12.3 
12.5 
12.6 
12.8 
13.0 

35 
36 
37 
38 
39 
40 
41 
42 
43 
44 
45 
46 
47 
48 
49 
50 
51 
52 
53 
54 
55 
56 
57 
58 
59 
60 
61 
62 
63 
64 
65 
66 
67 
68 
69 

13.1 
13.3 
13.4 
13.6 
13.8 
14.0 
14.2 
14.3 
14.5 
14.7 
14.9 
15.1 
15.3 
15.5 
15.6 
15.8 
16.0 
16.2 
16.4 
16.6 
16.8 
17.0 
17.2 
17.4 
17.6 
17.8 
18.0 
18.2 
18.4 
18.6 
18.8 
19.0 
1-9.2 
19.4 
19.6 

70 

71 
72 
73 
74 
75 
76 
77 
78 
79 
80 
81 
82 
83 
84 
85 
86 
87  « 
88 
89 
90 
91 
92 
93 
94 
95 
96 
97 
98 
99 
100 
101 
102 
102.25 

19.8 
20.0 
20.2 
20.4 
20.6 
20.8 
21.0 
21.2 
21.4 
21.6 
21.8 
22.0 
22.2 
22.4 
22.6 
22.8 
23.0 
23.2 
23.4 
23.6 
23.9 
24.1 
24.3 
24.5 
24.7 
25.0 
25.2 
25.5 
25.7 
25.9 
26.2 
26.4 
26.6 
26.75 

t°          K2SO4     Sp.  gr.  1        t°          KaSCU      Sp.gr. 

0.40      7.47  1.0589    58.95  18.01  1.1089 
15.70    10.37  1.0770    74.85  20.64  1.1157 
31.45    13.34  1.0921     89.70  22.80  1.1194 
42.75    15.51  1  .  1010|  101  .  1*  24.21  1.1207 

*=b.-pt. 
(Berkeley,  Phil.  Trans.  Roy.  Soc.  1904,  203. 
A,  189.) 

100  g.  H2O  dissolve  0.133  gram-equivalent 
K2SO4  at  25°    (Van't  Hoff  and  Meyerhoffer, 
Z.  phys.  Ch.  1904,  49.  315.) 
1  1.  sat  K2SO/+Aq  at  25°  contains  0.617 
mols.  K2SO4.  (Herz,  Z.  anorg.  1911,  73.  274.) 

Solubility  of  K2SO4  in  H2O  at  t°. 

t°                                     %  K2S04 

4.78                               7.82 
30.05                             11.43 
54.20                             14.77 
68.90                             16.40 

(Le  Blanc  and  Schmandt,  Z.  phys.  Ch.  1911, 
77.  614.) 

(  Mulder,  calculated  from  his  own  and  other 

If  solubility  S  =  pts.  anhydrous  salt  in  100 
pts.  of  solution,  S  =  7.5+0. 1070t  from  0°  to 
163°.  Solubility  from  163°  to  220°  is  constant 
at  25.  (Etard,  C.  R.  106.  208.) 


100  g.  H2O  dissolve  12.10  g.  K2SO4  at  25°. 
(Amadori,  Rend.  Ace.  Line.   1912,  (5)  21.  II. 

667.) 

Solubility  of  K2SO4  in  H2O  at  various  pres- 
sures. Figures  denote  pts.  K2SO4  con- 
tained in  100  pts.  sat.  K2SO4+Aq  at  t° 
and  A  pressure  in  atmospheres. 


t° 

Pts. 
K2S04 

t° 

Pts. 

K2S04 

t° 

Pts. 
K2S04 

A 

0° 

15° 

15.5° 

16.2° 

1 

20 
30 

6.81 
7.14 
7.14 

9.14 

9.24 
9.44 

9.35 
9.54 

16 
20 

28 
36 

9.76 
10.30 
12.59 
13.28 

39 
54 

98 

14.21 
17.39 
23.91 

120 
143 
170 

26.5 
28.8 
32.9 

(MSller,  Pogg.  117.  386.) 

(Tilden  and  Shenstone,  Phil.  Trans.  1884.  23.) 

Solubility  of  K2SO4  in  H2O.    100  pts.  H2O 
dissolve  at: 

4.3°         18.4°        69.9° 
8.16        10.8          19.7  pts.  K2SO4. 
(Andreae,  J.  pr.  (2)  29.  456.) 


Sat  K2SO4+Aq  boils  at  101.5°,  and  con- 
tains 26.33  pts.  K2SO4  to  100  pts.  H2O  (Gay- 
^ussac);  at  101.7°,  and  contains  21.2  pts. 
K2SO4  to  100pts.H2O  (Griffiths);  at  102.25°, 
and  contains  26.75  pts,  K2SO4  to  100  pts.  H2O 
Mulder);  boils  at  103°  (Kremers). 

Crust  forms  at  101.7°,  and  solution  con- 
tains 25.3  pts.  K2SO4  to  100  pts.  H2O;  highest 


1004 


SULPHATE,  POTASSIUM 


temp,  observed,  102.1°.     (Gerlach,  Z.  anal. 
26.  426.) 

B.-pt.  of  K2SO4+Aq  containing  pts.  K2SO4 
to  100  pts.  H2O. 


B.-pt. 

Pts.  K2SO4 

B.-pt. 

Pts.  K2S04 

100.5° 
101.0 
101.5 

7 
14.5 
22.1 

102° 
102.1 

30.0 
31.6 

(Gerlach,  Z.  anal.  26.  4300 


Sp.  gr.  of  K2SO4  at  19.5°. 


K2S04 


2.401 
4.744 
6.968 


gr. 


1.0193 
1  .  0385 
1  .  0568 


K2S04 


9.264 
10.945 


Sp.  gr. 


1.0763 
1  .  0909 


(Kremers,  Pogg.  95.  120.) 
Sp.  gr.  and  B-pt.  of  K2SO4+Aq  at  12.5°. 


Pts.  K2SO  to 
100  pts.  H2O 


Sp.  gr. 


1 . 0079 
1.0151 
1.0231 
1.0305 
1.0391 


B.-pt. 


100  .  38° 
100.63° 
100  .  75° 
100.88° 
101° 


2SO  to 
s.  H2O 


Sp.  gr. 


1.0456 
1.0524 
1.0599 
1.0676 
1.0735 


B.-pt. 


101.12° 
101.25° 
101.25° 
101.38° 
101  .  5° 


(Brandes  and  Gruner,  1827.) 

K2SO4-f-Aq  sat.   at  8°  has   1.072  sp.  gr 
(Anthon,  A.  24.  211.) 

K2SO4+Aq  saturated  at  12°  contains 
10.38%  K2SO4  and  has  sp.  gr.  1.0716  (Struve 
Zeit.  Ch.  (2)  6.  323);  saturated  at  15°  con- 
tains 11.01%  K2SO4  and  has  sp.  gr.  1.0831 
(Gerlach);  saturated  at  18.75°  contains 
10.74%  K2SO4  and  has  sp.  gr.  1.0798  (Kars- 
ten). 

Sp.  gr.  of  K2SO4+Aq  at  15°. 


Sp.  gr. 


1.0082 
1.0163 
1.0245 
1.0328 


Sp.  gr. 


1.0410 
1.0495 
1.0579 


8 
9 
9.92 


Sp.  gr. 


1.0664 
1.0750 
1.0830 


(Gerlach,  Z.  anal.  8.  287.) 
Sp.  gr.  of  K2SO4+Aq  at  18°. 


%K2S04 


5 

10 


Sp.  gr. 


1.0395 
1.0815 


(Kohlrausch,  W.  Ann.  1879.  1.) 


p.  gr.  of  K2SO4+Aq  at  15°/15°.  a  =  pts. 
K2SO4  in  100  pts.  of  the  solution;  b  =  pts. 
K2SO4  in  100  pts.  H2O. 


1 

3 
6 

7 
9 
9.92 


1.010 
3.093 
5.263 
7.527 
9.890 
11.013 


Sp.  gr. 


1.00808 
1.02447 
1.04091 
1.05776 
1.07499 
1.08305 


(Gerlach,  Z.  anal.  28.  493.) 

Sp.  gr.  of  K2SO4+Aq  at  20°  containing  0.5 
mol.    K2SO4    to    100    mols.    H2O  =  1.03758; 
:ontaining  1  mol.  K2SO4  to  100  mols.  H2O  = 
.06744.    (Nicol,  Phil.  Mag.  (5)  16.  122.) 

Sp.  gr.  of  K2SO4+Aq.  at  25°. 


Concentration  of  K2SO4 


1-nonnal 

Vr-      " 


Sp.  gr. 


1.0664 
1.0338 
1.0170 
1.0084 


(Wagner,  Z.  phys.  Ch.  1890,  6.  37.) 

K2SO4+Aq.  containing  6.7%  K2SO4  has 
sp.  gr.  20°/20°  =  1.0549.  (Le  Blanc  and 
Rohland,  Z.  phys.  Ch.  1896,  19.  278.) 

Sp.  gr.  of  K2SO4+Aq  at  20.1°,  when  p  = 
per  cent  strength  of  solution;  d  =  ob- 
served density;  w  =  volume  cone,  in 


gr.  per  cc. 


/pd_     \ 

•  ^100  ~wy 


p. 


9.83 

8.172 

6.779 

5.021 

3.127 

2.508 

1.448 

1.079 

1.047 

0.455 


d. 


,0800 
,0657 
,0539 
.0394 
.0238 
.0186 
.0100 
.0070 
.0066 


1.0018 


0.10615 
0.08708 
0.07144 
0.05218 
0.03202 
0.02554 
0.01463 
0.01087 
0.01053 
0.00456 


(Barnes,  J.  phys.  Chem.  1898,  2.  543.) 
Sp.  gr.  of  K2SO4+Aq  at  18°. 


Y<i  KzSO4  g.-equiv.  per  1. 

Sp.  gr.  at  18° 

0.8327 
0.7975 
0.6688 
0.5029 
0.5016 
0.2508 
0.01001 

1.0567 
1.0539 
1.0456 
1.0344 
1.0340 
1.0173 
1.0006 

(McKay,  Elektrochem.  Zeit.  1899,  6.  115.) 


SULPHATE,  POTASSIUM 


1005 


Sp.  gr.  of  sat.  K2SO4+Aq  at  t°. 


t° 

g.  K2SO4  sol.  in 
100  g.  H2O 

Sp.  gr. 

0 

7.35 

1.058 

10 

9.22 

1.069 

20 

11.11 

1.081 

30 

12.97 

1.089 

40 

14.76 

1.097 

50 

16.50 

1.106 

60 

18.17 

1.114 

70 

19.75 

1.121 

(Tschernaj,  J.  Russ.  phys.  Chem.  Soc.  1912, 
44.  1565.) 

Sol.  in  cone,  acids;  not  pptd.  by  glacial 
HC2H3O2.  Insol.  in  KOH+Aq  of  1.35  sp.  gr. 
(Liebig,  A.  11.  262.) 

Solubility  of  K2SO4  in  H2SO4-f  Aq  at  18°. 


Mols.  per  100  mols. 

solution 

Solid  phase 

K2SO4 

H2SO4 

1.10 

0 

K2S04 

1.59 

0.95 

1C 

2.49 

2.70 

It 

2.75 

3.17 

K2SO4,  KHSO4 

2.75 

3.74 

{{ 

2.83 

5.08 

tt 

2.80 

5.79 

K2S04,  3KHS04 

2.61 

5.61 

K2S04,  6KHS04 

2.25 

6.19 

"  +KHS04 

1.08 

7.94 

KHS04 

0.77 

9.2 

t( 

0.44 

22.7 

(t 

(Stortenbecker,  R.  t.  c.  1902,  21.  407.) 
Solubility  in  H2SO4+Aq  at  0°. 


1000  g.  of  the  solution 
contain 

Solid  phase 

Mols 
H2S04 

Mols 
K2S04 

0.393 

K2S04 

0^37 

0.53 

u 

0.75 

0.64 

!t 

.08 

0.74 

K2S04+K3H(S04)2  • 

.13 

0.73 

K3H(S04)2 

.44 

0.71 

u 

.66 

0.69 

tt 

.89 

0.66 

K3H(SO4)2+Ka 

.88 

0.69 

u 

2.15 

0.59 

Ka+Kb 

2.12 

0.61 

14 

2.29 

0.54 

Kb 

2.30 

0.53 

Kb+KHSO4 

2.33 

n 

2.48 

0^43 

KHS04 

3.08 

0.28 

" 

4.43 

0.12 

tt 

5.27 

0.09 

u 

These  results  show  that  at  0°  there  exist 


between  K3H(SO4)2  and  KHSO4,  two  acid 
sulphates,  Ka  and  Kb.  Ka  is  probably 
K2SO4,  3KHSO4  and  Kb  is  probably  K2SO4, 
6KHSO4. 

(D'Ans,  Z.  anorg.  1909,  63.  228.) 


3.1  mols.  K2SO4  are  sol.  in  absolute  H2SO4 
at  25°.    (Bergius,  Z.  phys.  Ch.  1910,  73.  353.) 


Solubility  in  H2SO4+Aq  at  25°. 


Millimols  H2SO4 
in  10  com. 

Millimols  K2SO4 
in  10  com. 

3^97 
7.57 
14.35 

6.17 
8.92 
10.82 
14.86 

(Herz,  Z.  anorg.  1912,  73.  276.) 


Solubility  in  H2SO4+Aq  at  25°. 


In  1000  g.  of 
the  solution 

Solid  phase 

Mols 
SO3 

Mols 
K2SO4 

6.42 

0.171 

KHSO4 

6.60 

0.190 

« 

6.91 
7.26 

0.266 
0.182 

KHSO4+KH3(SO4)2,  H2O 

7.62 

0.157 

U 

7.88 

0.167 

tt 

8.00 

0.201 

« 

8.10 

0.250 

KH3(S04)2,  H20 

8.15 

0.352 

n 

8.16 

0.364 

KH3(S04)2,  H20+KH3(S04)2 

8.29 

0.341 

« 

8.33 

0.322 

« 

8.45 

0.325 

u 

8.62 

0.346 

(( 

8.57 

0.384 

KH3(S04)2 

8.71 

0.412 

(i 

8.82 

0.583 

KH3(S04)2 

8.65 

0.880 

KH3(SO4)2+KHS2O7 

8.63 

0.899 

KHS2O7(metastable  solution) 

8.70 

0.882 

« 

8.96 

0.561 

I  .61?   ,)  5  '•                     (' 

9.80 

0.365 

n 

9.78 

0.430 

tt 

9.80 

0.665 

KHS207 

9.66 

0.904 

ft 

9.66 

0.937 

K 

(D'Ans,  Z.  anorg.  1913,  80.  239.) 


Pptd.  from  K2SO4+ Aq  by  NH4OH+Aq. 
(Sullivan.) 


1006 


SULPHATE,  POTASSIUM 


Solubility  of  K2SO4  in  NH4OH+Aq  at  20°. 

Solubility  of  K2SO4  in  Na2SO4+Aq. 

G.  NH3  in 
100  ccm.  H2O 

G.  K2SO4  in 
100  ccm.  H2O 

Temp.  =34° 

Temp.  =60° 

%  Na2S04 

%  K2S04 

%  Na2S04 

%  K2S04 

0 
6.08 

15.37 
24.69 
31.02 

10.801 
4.100 

0.828 
0.140 
0.042 

0 
7.1 
31.4 
33.1 

11.9 
10.7 
4.3 
0 

0 
6.6 
27.1 
31.3 

15.3 
13.9 

8.2 
0 

(Girard,  Bull.  Soc.  (2)  43.  522.) 


1  1.  sat.  solution  in  H2O  contains  105.7  g. 
K2SO4  at  20°;  in  NH4OH+Aq  (5.2%  NH3), 
45.2  g.  (Konowalow,  J.  Russ.  Phys.  Chem. 
Soc.  1894,  31.  985.) 


(Nacken,  B.  A.  B.  1910.  1016.) 

100  g.   H2O   sat.   with  both  K2S04   and 
T12SO4  dissolve: 

'  4.74  g.  T12SO4+10.3  g.  K2SO4  at   15°. 
11.5  g.        "      +16.4  g.      "      ."     62°. 
18.52  g.      "      +26.2  g.      "       "  100°. 
(Rabe,  Z.  anorg.  1902,  31.  156.) 


Solubility  of  K2SO4  in  KOH+Aq  at  25°. 

SI.  sol.  in  sat.  ZnSO4  or  CuSO4+Aq  with 
separation  of  double  salt. 
100    pts.    H2O    dissolve    8.5+0.12t    pts. 
K2SO4.     On  addition  of  a  K  salt,  K2SO4  is 
pptd.     The  amount  of  K2SO4  remaining  in 
solution  plus  the  amt.  of  K  in  the  salt  added 
is  a  constant.    (Blarez,  C.  R.  112.  939.) 

Solubility  of  K2SO4+Th(SO4)2  at  16°. 
Solid  phase,  Th(SO4)2. 

In  1000  g.  of  the  solution 

Mols  K2S04 

Mols  (KOH)2 

0.617 
0.433 
0.280 
0.137 
0.035 
0.009 
0.0 

0.0 
0.258 
0.433 
1.13 
2.86 
3.42 
4.809 

Pts.  per  100  pts  H2O 

Pts.  per  100  pts.  H2O 

K2SO4 

Th(SO4)2 

KzSO4 

Th(S04)2 

0.000 
0.424 
1.004 
1.152 
1.224 
1  .283 
1.348 
1.378 

1.390 
1.667 
2.193 
3.191 
2.514 
2.222 
1.706 
1.637 

1.487 
1.633 
1.844 
2.512 
3.092 
4.050 
4.825 

0.870 
0.635 
0.370 
0.128 
0.070 
0.027 
0.003 

(D'Ans  and  Schreiner,  Z.  anorg.   1910,   67. 

438.) 

Sol.  in  sat.  NH4Cl+Aq  without  pptn.    (See 
NH4C1.) 
SI.   sol.   in   sat.   KCl+Aq  without   pptn. 
inn  «•  oof  T^niJ-An    of  o^0  ^oa^itra  n  niA7 

g.  equiv.  K2SO4  at  25°.  (Van't  Hoff  and 
Meyerhoffer  Z.  phys.  Ch.  1904.  49.  315.) 

SI.  sol.  in  sat.  KNOa+Aq  without  causing 
pptn. 

1 1.  of  the  solution  contains  50.7  g.  K2SO4+ 
216.5  g.  KN08=267.2  g.  mixed  salts  at  15°. 
Sp.  gr.  K2SO4+KNO8+Aq  =  1.165. 

1 1.  of  the  solution  contains  47.66  g.  K2SO4 
+308.5  g.  KNO3  =  356.2  g.  mixed  salts  at 
25°.  Sp.  gr.  of  K2SO4+KN08+Aq  =  1.210. 
(Euler,  Z.  phys.  Ch.  1904,  49.  313.) 

See  also  under  KNO8. 

Sol.  in  sat.  NaNOs+Aq  without  causing 
pptn  at  first,  but  soon  KNOs  is  pptd.  (Kar- 
sten.)  (See  NaNO3.) 

Sol.  in  (NH4)2SO4+Aq  with  pptn.  of 
(NH4)2SO4.  (Rudorff,  B.  6.  485.)  (See 
(NH4)2S04.) 

More  sol.  in  aqueous  solutions  of  other  salts, 
as  Na2SO4,  MgSO4,  CuSO4,  etc.,  than  in  pure 
H2O.  (Pfaff,  A.  99.  227.) 

Sol.  in  sat.  Na2SO4+Aq,  MgSO4+Aq, 
NaCl+Aq.  (See  MgSO4  and  NaCl.) 


(Barre,  C.  R.  1911,  150.  1555.) 

Difficultly    sol.    in    20%    KC2H3O2+Aq. 
(Stromeyer.) 

Solubility  in  K  acetate +Aq  at  25°. 


'  *  V*£          Composition  of  the  solutions 

%  K  acetate 

%  K2S04 

%H20 

6.11 
8.68 
11.29 
15.59 
20.12 
29.95 

6.65 
5.09 
3.99 
2.35 
1.23 
0.39 

87.24 
86.23 
84.72 
82.06 
78.65 
69.66 

The  solid  phase  in  these  solutions  is  K2SO4. 
(Fox,  Chem.  Soc.  1909,  95.  885.) 

100  g.  hydroxylamine  dissolve  3.5  g. 
K2SO4  at  17-18°.  (de  Bruyn,  Z.  phys.  Ch. 
1892,  10.  782.) 


SULPHATE,  POTASSIUM 


1007 


Easily   sol.    in  liquid  HF.      (Franklin,    Z. 

Solubility  in  organic  substances  +Aq  at  25°. 

anorg.  1905.  46.  2) 

Insol.  in  liquid    NH3.       (Franklin,     Am. 

Composition  of  the  solutions 

Ch.  J.  1898,  20.  829.) 
Neither  dissolved  nor  attacked  by  liquid 
NO2.      (Frankland,     Chem.   Soc.    1901,   79. 

Organic  substance 

%  organic 
substance 

%  K2SO4 

%  H20 

1361.) 
Insol.  in  absolute  alcohol. 
Insol.  in  alcohol,  the  sp.  gr.  of  which  is 
0.905.     (Anthon.) 
Solubility  in  dil.  alcohol  increases  with  the 

tjGHlD 

Alcohol 

1.35 

4.80 
7.80 
9.70 
12.34 

9.17 
6.90 
4.96 
4.32 
3.57 

89.48 
88.30 
87.24 
85.98 
84.09 

100  pts.  alcohol  of  0.939  sp.  gr.  (53%  by 
vol.,  45%  by  weight)  dissolve  at: 

14.51 
15.26 
20.50 

2.71 
2.66 
1.83 

82.78 
82.08 
77.67 

4°           8°           60° 
046        0.21        0.92  pts.  K2SO4. 

26.91 
35.97 

0.97 
0.41 

72.12 
63.62 

(Gerardin,  A.  ch.  (4)  6.  147.) 

43.90 

0.22 

55.88 

100  pts.  of  the  sat.  solution  at  15°  in  alcohol 

69.26 

0.016 

30.72 

of: 

10       20        30         40%  by  weight, 
contain  3.9      1.46      0.56      0.21  pts.  K2SO4. 
(Schiff,  A.  118.  362.) 

Pyridine 

4.23 
13.90 
24.51 
34.19 

7.95 
4.77 
2.75 
1.47 

87.82 
81.33 
72.74 
64.34 

Solubility  in  acetic  acid+Aq  at  25°. 

46.29 

r  e    r\o 

0.45 

01  O 

53.26 

A  O      f\f 

Concentration  of  the 
acetic  acid  Mol./Liter 

Solubility  of  K2SO4 
Mol./Liter 

55.93 
75.90 

.  12 
0.006 

43.95 
24.09 

0.000 

0.6714 

Ethylene  glycol 

3.16 

9.67 

87.17 

0.070 

0.6619 

9.89 

7.69 

82.53 

0.137 

0  .  6559 

18.47 

5.74 

75.79 

0.328 

0.6350 

32.11 

3.57 

64.32 

0.578 

0.6097 

49.03 

1.83 

49.14 

1.151 
2.183 

0.5556 
0.4743 

Chloral  hydrate 

6.44 

9.13 

84.43 

9.09 

8.41 

82.50 

(Rothmund  and  Wilsmore,  Z.  phys.  Ch.  1902 

12.38 

7.79 

79.83 

40.  620.) 

13.20 

7.31 

79.49 

Solubility  in  phenol  +Aq  at  25°. 

22.07 
33.  15 

5.88 

4    f)A 

72.05 
62  31 

Concentration  of  the 

Solubility  of  K2SC>4 

44.40 

TT  .  «_|T: 

3.36 

\j&  .  O  J. 

52.24 

phenol  Mol/Liter 

Mol/Liter 

47.30 

2.92 

49.78 

0.000 
0.016 
0.021 
0.032 

0.6714 
0.6650 
0.6614 
0.6598 

62.82 

70.28 
80.36 
85.26 

2.00 
1.75 
1.40 
1.08 

35.18 
27.97 
18.24 
13.66 

0.040 
0.047 

0.6555 
0.6522 

Glycerol 

8.96 

1Q    QA 

8.87 
7  fiQ 

82.17 

70     QK 

0.064 

0.6502 

-LO  .  OvJ 

20.34 

t    .  \J\J 

6.47 

9  O  .  i/O 

73.19 

0.076 
0.127 
0.152 
0.236 
0.252 

0  .  6494 
0.6310 
0.6251 
0.6042 
0.5956 

24.15 
33.73 
40.40 
43.52 
50.  18 

5.83 
4.44 
3.65 
3.38 
2  fiQ 

70.02 
61.83 
55.95 
53.10 
47   13 

0.308 

0.5834 

57^22 

^i  .  U*7 

2.07 

^  *   .  J.O 

40.71 

0.409 
0.464 
0.486 
0.495 

0  .  5572 
0.5480 
0.5425 
0.5389 

67.94 

78.18 
98.28 

1.53 
0.98 
0,73 

30.53 
20.84 
0.99 

0.498  (saturated) 

0.5377 

Mannitol 

3.20 

10.32 

86.48 

(Rothmund  and  Wilsmore,  Z.  phys.  Ch.  1902 

5.82 

10.07 

84.11 

40.  619.) 

8.35 

9.61 

82.04 

100  g.  95%  formic  acid  dissolve  36.5  g 
'    K2SO4  at  21°.     (Aschan,  Ch.  Ztg.  1913,  37 
1117.) 

11.26 
14.30 
17.22 

9.19 
8.66 
8.35 

79.55 
77.04 
74.43 

1008 


SULPHATE,  POTASSIUM  HYDROGEN 


Solubility  in  organic  substances  +Aq  at  25°.  — 
Continued. 

Insol.  in  methyl  acetate.      (Naumann  B. 
1909,  42,  3790.) 
Min.  Misinite. 
+5j^H2O.     Deliquescent.        (Senderens, 
Bull.  Soc.  (3)  2.  278.) 

Potassium  cfthydrogen  sulphate,  K^^SO^s. 
Sol.  in  H2O.     (Phillips,  Phil.  Mag.  1.  429.) 
Composition  is  4K20,  7SO3+3H2O,  accord- 
ing to  Berthelot  (A.  ch.  (4)  30.  442). 

Potassium  frihydrogen  sulphate,  KH8(SO4)2. 

Sol.    in    H2O    with    rise    of    temperature. 
(Schultz,  Pogg.  133.  137.) 
+  1HH2O.     (Lesco3ur,  C.  R.  78.  1044.) 

Potassium  cfo'sulphate  (p?/rosulphate),  K2S207. 
When  dissolved  in  exactly  the  necessary 
amount  of  hot  H2O  for  solution,  it  crystallises 
on  cooling  without  decomp.     Decomp.   by 
excess  of  H2O.     (Jacquelain,  A.  ch.  70.  311.) 
Insol.  in  methyl  acetate.     (Naumann,  B. 
1909.  42.  3790.) 

Organic  substance 

Composition  of  the  solutions 

%  organic 
substance 

%  K2S04 

%H20 

Sucrose 

9.56 
18.55 
28.16 
37.24 
47.55 
57.00 

9.65 
8.65 
7.42 
6.35 
5.21 
4.24 

80.79 
72.80 
64.42 
56.41 
47.24 
38.76 

Acetone 

4.92 
10.06 
16.23 
24.31 
37.19 
46.29 
62.40 

7.20 
5.02 
2.96 
1.50 
0.47 
0.20 
0.03 

87.88 
84.92 
80.81 
74.19 
62.34 
53.51 
37.57 

(Fox  and  Gage,  Chem.  Soc.  1910,  97.  381.) 

Sol.  in  76  pts.  glycerine  of  1.225  sp.  gr.  at 
ordinary  temp.  (Vogel,  N.  Repert.  16.  557.) 

Insol.  in  acetone.  (Krug  and  M'Elroy; 
Eidman,  C.  C.  1899,  II.  1014.) 

Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.257);  benzonitrile.  (Naumann,  B.  1914, 
47.  1370);  methyl  acetate.  (Naumann,  B. 
1909,  42,  3790);  ethyl  acetate.  (Naumann. 
B.  1904,  37,  3602.) 

100  g.  H2O  dissolve  104  g.K2SO4+219.0 
g.  sugar  at  31.25°,  or  100  g.  sat.  solution  con- 
tain 3.8  g.  K2SO4 +66.74  g.  sugar.  (Kohler, 
Z.  Ver.  Zuckerind.  1897,  47.  447.) 

Min.  Glaserite. 

+  i^H2O.  100  pts.  H2O  dissolve  9.82  pts. 
(Ogier,  C.  R.  82.  1055.) 

Tn'potassium  hydrogen  sulphate,  K8H(S04)2. 
Sol.  in  H2O. 

Potassium  hydrogen  sulphate,  KHSO4. 
1.07  pts.  KHSO4  (  =  1  pt.  K2S2O7)  dissolve: 
at    0°  in  2.95  pts.  H2O. 
"    20°  "2.08        " 
"    40°  "  1.59        " 
"  100°   "  0.88        " 
(Kremers,  Pogg.  92.  497.) 

Sp.  gr.  of  KHSO4+Aq  at  15°  containing: 
5  10  15  %  KHSO4, 

1.0354     1.0726     1.1116 

20          25  27%    KHS04. 

1.1516     1.1920     1.2110 
(Kohlriiusch,  W.  Ann.  1879.  1.) 

Sat.  solution  boils  at  105.5°  (Griffiths); 
108°  (Kremers). 

Alcohol  dissolves  out  H2SO4. 

K2SO4   crystallises   from    dilute   solutions. 

100  g.  95%  formic  acid  dissolve  14.6  g. 
KHSO4  at  19.3°.  (Aschan,  Ch.  Ztg.  1913,  37. 
1117.) 


Potassium  hydrogen  ^'sulphate,  KHS2Oy. 

Sol.  in  fuming  H2SO4  without  decomposi- 
tion. 

Potassium  odosulphate,  K2S8O26. 
Decomp.  by  H2O.     (Weber.) 

Potassium  praseodymium  sulphate,  3K2S04, 
Pr2(S04)8+H20. 

SI.  sol.  in  H2O. 

Sol.  in  cone.  HC1  and  HNO3.  (Von  Scheele 
Z.  anorg.  1898,  18.  358.) 

Potassium  rhodium  sulphate,  3K2SO4, 

Rh2(S04)8. 

Does  not  exist.     (Leidie,  C.  R.  107.  234.) 
K2SO4,  Rh2(SO4)3+24H2O.     Very  sol.  in 
H2O.    (Piccini,  Z.  anorg.  1901,  27.  66.) 

Potassium  samarium  sulphate,  9K2SO4, 
2Sm2(S04)8+3H20. 

SI.  sol.  in  H2O. 

SI.  sol.  in  sat.  K2SO4+Aq. 

1  1.  sat.  K2SO4+Aq  dissolves  0.5  g.  Sm2O3. 
(Cleve,  Bull.  Soc.  (2)  43.  166.) 

Potassium  scandium  sulphate,  3K2S04, 

Sc2(S04)3. 

Very  slowly  sol.  in  cold,  more  easily  sol. 
in  warm  H2O.  Insol.  in  sat.  K2SO4+Aq. 

Sol.  in  H2O  and  in  dil.  K2SO4  + Aq.  (Meyer, 
Z.  anorg.  1914,  86.  279.) 

2K2SO4,  Sc2(SO4)3.  Sol.  in  K2SO4+Aq. 
(Cleve.) 

Does  not  exist.     (Nilson.) 

Potassium  sodium  sulphate,  3K2S04,  Na2SO4. 

100  pts.  H2O  dissolve  40.8  pts.  at  103.5°. 
(Penny,  Phil.  Mag.  (4)  10.  401.) 

5K2SO4,  Na2SO4.  100  pts.  H2O  at  100° 
dissolve  25  pts.  ;  at  12.7°,  10.1  pts.  ;  at  4.4°, 
9.2  pts.  (Gladstone,  Chem.  Soc.  6.  111.) 


SULPHATE,  POTASSIUM  YTTRIUM 


1009 


Potassium  strontium  sulphate,  K2Sr2(SO4)2. 

Decomp.  by  (NH4)2CO3+Aq.  (Rose. 
Pogg.  93.  604.) 

K2SO4,  SrSO4.     This  is   the   only   double 
salt    formed    from   these  two    components 
between  0°  and  100°. 

100  pts  of  the  sat.  solution  in  equilibrium 
with  SrSO4  and  the  double  salt  contain  at: 
17.5°      50°       75°      100° 
1.27      1.88     2.71      3.9  pts.  K2SO4. 
(Barre,  C.  R.  1909,  149.  292.) 

Potassium  tellurium  sulphate,  KHS04,  2TeO2, 

S08+2H20. 
(Metzner,  A.  ch.  1898,  (7)  16.  203.) 

Potassium  terbium  sulphate. 

Easily  sol.  in  H2O.  SI.  sol.  in  K2SO4+Aq. 
(Delafontaine,  Zeit.  Chem.  (2)  2.  230.) 

Potassium  thallic  sulphate,  KT1(SO4)2+ 
4H2O. 

Decomp.  by  H2O.  (Fortini,  Gazz.  ch. 
it.  1905.  36.  (2)  453.) 

2K2O,  T12O3,  4SO3.  Insol.  in  H2O.  Very 
difficultly  sol.  in  warm  dil.  H2SO4+Aq. 
(Strecker,  A.  135.  207.) 

Potassium  thorium  sulphate,  K2S04,  Th(S04)2 
+4H20. 

Sol.  in  hot  H2O  containing  a  few  drops 
HC1.  (Barre,  A  ch.  1911,  (8)  24.  227.) 

2K2SO4,  Th(SO4)2+2H2O.  Slowly  sol.  in 
cold,  easily  and  abundantly  in  hot  H2O, 
and  is  gradually  decomp.  by  boiling.  Easily 
sol.  in  acids.  Insol.  in  alcohol.  (Berzelius.) 

3.5K2SO4,  Th(SO4)2.  Insol.  in  K2SO4+Aq 
of  con2entrations  above  4.5%.  (Barre.) 

4K2SO4,    Th(SO4)2+2H2O.      (Chydenius.) 

Potassium  tin  (stannous)  sulphate,  K2SO4, 

SnS04. 
(Marignac.) 

Potassium  tin  (stannic)  sulphate,  K2Sn(SO4)8. 

Easily  sol.  in  H2O  with  decomp. 

Sol.  in  HC1.  (Weinland,  Z.  anorg.  1907, 
64.  250.) 

Potassium  tin  (stannous)  sulphate  chloride, 

4K2S04,  4SnS04,  SnCl2. 
Can  be  recrystallised  from  H2O.     (Marig- 
nac, Ann.  Min.  (5)  12.  62.) 

Potassium  titanium  sulphate,  K2S04,  Ti(SO4)2 
+3H2O. 

Difficultly  sol.  in  H2O  or  HCl+Aq.  De- 
comp. by  much  H2O.  (Wallace,  Pogg.  102. 
453.) 

Potassium  titanyl  sulphate,  2K2SO4,   3TiO, 

SO4+10H2O. 

Very  sol.  in  H2O  with  decomp.     Insol.  in 

cone.  H2SO4.      (Rosenheim,  Z.  anorg.  1901, 

26.  251. 


K2S04,  Ti02S04+7H20.  Very  hygro- 
scopic and  sol.  in  H2O.  (Mazzuchelli  and 
Pontanelli,  C.  C.  1909,  II.  420.) 

K2S04,(TiO)S04.    (Spence,  C.  C.  1901,  II. 

Potassium  uranous  sulphate,  K2SO4,  U(S04)» 
+H20. 

Very  si.  sol.  in  H2O.    (Rammelsberg.) 

Potassium  uranyl  sulphate,  K2SO4,  (U02)S04 
+2H20. 

Sol.  in  9  pts.  H2O  at  22°  and  in  0.51  pt.  at 
100°.  Insol.  in  alcohol.  (Ebelmen,  A.  ch. 
(3)  5.  211.) 

100  pts.  of  aqueous  solution  sat.  at  25° 
contain  10.5  pts.  salt;  at  70.5°  contain  23.93 
pts.  salt.  (Rimbach,  B.  1904,  37.  478.) 

+3H2O.  (de  Coninck,  Chem.  Soc.  1905, 
88.  (2)  394. 

2K2SO4,  (UO2)SO4+2H2O.  Decomp.  by 
H20. 

Cannot  be  cryst.  from  rather  cone.  H2S04, 
as  it  is  completely  decomp.  by  it.  (Rimbach, 
B.  1905,  38.  1572.) 

K2O.  2UO3,  3SO3.  Ppt.  Identical  with 
UO2,  OK,  SO3H  of  ScheUer,  (A.  1867,  144. 
238.)  (Kohlschutter,  A.,  1900,  311.  11.) 

2K2SO4,  3(UO2)SO4+H2O.  Sol.  in  H20. 
Insol.  in  alcohol.  (Berzelius.) 

Does  not  exist.    (Ebelmen.) 

Potassium  vanadium  sulphate,  K20,  V2O«, 

2SO3+6H2O  =K(VO2)SO4+3H2O. 

(Friedheim,  B.  24.  1183.) 

=KVO3,  K2SO4,  V2O5,  2SO3+9H2O  of 
Miinzing  (Berlin,  Dissert.  1889). 

K2S04,  VS04+6H20.  Sol.  in  H20.  (Pic- 
cini,  Z.  anorg.  1902,  32.  61.) 

K2V2(SO4)4+24H2O.  100  pts.  H2O  dis- 
solve 198.4  pts.  salt,  at  10°.  Sp.  gr.  of  sat. 
solution  at  4°/20°  =  1.782.  (Piccini,  Z.  anorg. 
1897,  13.  446.) 

Potassium  vanadyl  sulphate, 
K2S04,  (VO)2(S04)3. 

Very  slowly  sol.  in  H2O,  still  less  sol.  in  dil. 
alcohol.  (Gerland.) 

K2SO4,  VOSO4+3H2O.    Easily  sol.  in  H20. 

Sol.  in  alcohol+conc.  H2SO4.  (Koppel, 
Z.  anorg.  1903,  36,  178.) 

K2SO4,  2VOSO4.  Very  hygroscopic.  Very 
sol.  in  H2O  but  goes  into  solution  slowly. 
(Koppel  and  Behrendt,  B.  1901,  34.  3935.) 

Easily  sol.  in  H2O.  (Koppel,  Z.  anorg. 
1903,  36.  174.) 

Potassium  yttrium  sulphate,  4K2S04, 

Y2(S04)8. 

Sol.  in  16  pts.  cold  H2O,  and  in  10  pts.  sat. 
K2SO4+Aq,  and  more  abundantly  if  the  latter 
solution  contains  ammonium  salts  or  free 
acid.  (Berlin.) 

3K2SO4,   2Y2(SO4)3.     100   ccm.   cold  sat. 


1010 


SULPHATE,  POTASSIUM  ZINC 


K2SO4+Aq  dissolve  an  amount  of  this  salt 
corresponding  to  4.685  g.  Y2O3.    (Cleve.) 

Potassium  zinc  sulphate,  K2SOi.  ZnSO4+ 
6H20. 

Sol.  in  5  pts.  cold  H2O.  (Bucholz,  N.  J.  Pharm.  9. 
2.  26.) 

100  pts.  H2O  dissolve  at: 
0°      10°     15°     25°     36° 
12.6   18.7  22.5   28.8   39.9  pts.  hydrous  salt, 

45°     50°    58°     65°     70° 
51.2   54.0   67.6   81.3    87.9  pts.  hydrous  salt. 
(Tobler,  A.  95.  193.) 

100  pts.  H20  at  15°  dissolve  14.8  pts.  K2SO4, 
ZnSO4+6H2O;  sp.  gr.  of  sat.  H2O  solution  at 
15°  =  1.0939.  (Schiff,  A.  109.326.) 

1  1.  H2O  dissolves  131.9  g.  anhydrous 
salt  at  25°.  (Locke,  Am.  Ch.  J.  1902,  27. 
459.) 

Potassium  zirconium  sulphate,  2K2O,  6ZrO2| 

7S03+9H20. 
Decomp.  by  H2O. 

3K2O,  3ZrO2,  7SO3+9H2O.    Insol.  in  H2O. 
Zr2O3(KSO4)2+8H2O.     Ppt.     (Rosenheim, 
B.  1905,  38.  815.) 


Potassium  sulphate  vanadate. 

Very   difficultly   sol.   in   H2O. 
alcohol.    (Berzelius.) 


Insol. 


Potassium  sulphate  antimony  Jn'fluoride. 

See    Antimony  Irifluoride  potassium  sul- 
phate. 


Praseodymium  sulphate,  basic,  (PrO)2SO4. 

Insol.  in  H2O.  (Matignon,  C.  R.  1902, 
134.  660.) 

Insol.  in  H2O.  Nearly  insol.  in  dil.  acids. 
(Wohler,  B.  1913,  46.  1730.) 


Praseodymium  sulphate,  Pr2(SO4)8. 

Sol.  in  H2O;  very  hydroscopic.  23.64  pts. 
are  sol.  in  100  pts.  H2O  at  0°  and  17.7  pts.  at 
20°.  (von  Scheele,  Z.  anorg.  1898,  18.  357- 
358.) 

+5H2O.  Sol.  in  H2O.  (von  Scheele,,  Z. 
anorg.  1898,  18.  357.) 

Difficultly  sol.  in  H2O.  (Kraus,  Zeit. 
Kryst.  1901,  34.  400.) 

1.50  pts.  Pr2(SO4)3  are  sol.  in  100  pts.  H2O 
at  85°;  1.45  pts.  at  90°;  and  1.02  pts.  at  95°. 
(Muthmann  and  Rolig,  B.  1898,  31.  1729.) 

+8H2O.  (Kraus,  Zeit.  Kryst.  1901,  34. 
406.) 

Sol.  in  H2O.  (von  Scheele,  Z.  anorg.  1898, 
18.  357.) 


Solubility  in  H2O  at  t°. 


t 

Pts.  Pr2(SO4)3 

0 

18 
35 
55 
75 

19.79 
14.10 
10.31 
7.09 
4.13 

(Muthmann  and  Rolig,  B.  1898,  31.  1727.) 

+15HH2O.     Sol.  in  H2O.     (von  Scheele, 
Z.  anorg.  1898,  18.  357.) 

Praseodymium  hydrogen  sulphate,  Pr(S04H)8. 

(Brauner,  Z.  anorg.  1904,  38.  330.) 

Solubility  in  boiling  cone.  H2SO4.     100  g, 

of  the  solution  contain  1.02  g.  of  the  acid 

sulphate.     (Matignon,  C.  R.  1902,  134.  659.) 

Radium  sulphate. 

Less  sol.  in  H2O  than  corresponding  Ba 
comp.    (Curie,  Dissert.  1903.) 


Rhodium  sulphate,  Rh2(SO4)8+12H20. 
Easily  sol.  in  H2O.    (Berzelius.) 
SI.  sol.  in,  but  not  decomp.  by  H2O  when 

not  more  than  16  pts.  H2O  are  present  to  1 

pt.  salt.    Decomp.  by  hot  H2O  to — 
Rh2(SO4)3,Rh2O3.    Insol.  in  H2O.    (Leidid, 

C.  R.107.  234.) 

Rhodium    rubidium     sulphate,     Rh2(S04)3, 

Rb2SO4+24H2O. 

Sol.  in  H2O;  m.-pt.,   108-109°.     (Piccini, 
Z.  anorg.  1901,  37.  65.) 

Rhodium  thallium  sulphate,  Rh2(S04)3)  T12S04 

+24H2O. 

Very  sol.  H2O.     (Piccini,  Z.  anorg.  1901, 
37.  69.) 


Rhodium  sodium  sulphate,  Rh2Na2(S04)4. 

Insol.  in  H2SO4  or  aqua  regia.     (Seubert 
and  Kobbe,  B.  23.  2560.) 

Rubidium  sulphate,  Rb2S04. 

100  pts.  H2O  dissolve  42.4  pts.  at   10°. 
(Bunsen.) 

100  cc.   H2O   at   17-18°   dissolve  44.7  g. 
Rb2SO4.    (Tutton,  Chem.  Soc.  1894,  65.  632.) 
Sat.  Rb2SO4+Aq  contains  at: 
3°          20° 
27.4        32.5%  Rb2S04, 

37°       [97°         170° 
37.3       43.9     "  49.2%  Rb2SO4. 
(fitard,  A.  ch.  1894,  (7)  2.  550.) 


SULPHATE,  SAMARIUM 


1011 


SolubUity  of  Rb2SO4  in  H2O  at  t°. 

Insol.  in  H2O.     Sol.  in  HC1.     Insol.  in 
H2SO4.      Decomp.    by    boiling    with    cone. 
H2S04.    (Stabler,  B.  1905,  38.  2623.) 

Rubidium  uranyl  sulphate,  Rb2(U02)(S04)2+ 
2H20. 
Somewhat  less  sol.  in  H2O  than  K   salt. 
(Rimbach,  B.  1904,  37.  479.) 

Rubidium  vanadium  sulphate.  Rb2V2(SO4)4+ 
24H20. 

n  177     rrram     mr»la       f\f     a  n  Vi  \rr\  rm  l  <a     <aalt.     flTP 

t° 

g.Rb2SO4perlOOg 

t° 

g.  RbzSChperlOOg. 

H2O 

solution 

H20 

solution 

0 
10 
20 
30 
40 
50 

36.4 
42.6 
48.2 
53.5 
58.5 
63.1 

27.3 
29.9 
32.5 
34.9 
36.9 
38.7 

60 
70 
80 
90 
100 
102.4* 

67.4 

71.4 
75.0 

78.7 
81.8 
82.6 

40.3 
41.7 
42.9 
44.0 
45.0 
45.2 

*  -ts.-pt.  at  Y42.4  mm. 
(Berkeley,  calc.  by  Seidell,  Solubilities,  2nd 
Ed.,  p.  587.) 

Sp.  gr.  of  Rb2SO4+Aq  sat.  at  10°  =  1.2978. 
(Erdmann,  Arch.  Pharm.  1894,  232.  16.) 


G.-equiv.  salt  per  1.  at  18° 
Sp.  gr.  6°/6° 

"      18718° 

"      30°/30° 


0.501  1.01 

1.05587  1.11047 

1.05496  1.10896 

1.05433  1.10810 


G.-equiv.  salt  per  1.  at  18°=  2.043       3.168 
Sp.gr.  6°/6°  1.21888    1.33276 

"      18718°  1.21613    1.32912 

"      30°/30°  1.21443    1.32750 

(Clausen,  W.  Ann.  1914,  (4)  44.  1071.) 

10  ccm.  of  sat.  Rb2SO4+ absolute  H2SO4 
mtain  approx.  5.881  g.  R 
Z.  phys.  Ch.  1910,  72.  355.) 


contain  approx.  5.881  g.  Rb2SO4.     (Bergius, 
",  phys.  Ch.  1910,  72.  355.) 

Insol.   in  methyl   acetate    (Naumann,   B. 


1909,  42.  3790);  acetone  (Naumann,  B.  1904, 
37.  4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Rubidium  p?/rosulphate,  Rb2S2O7. 
Decomp.  by  H2O. 

Rubidium  ocfosulphate,  Rb2S8025. 
Decomp.  by  H2O.     (Weber,  B.  17.  2497.) 

Rubidium  hydrogen  sulphate,  RbHSO4. 

Sol.  in  H2O. 

Rubidium  tin  (stannic)  sulphate,  Rb2Sn(SO4)3. 
Decomp.  by  H2O.     Sol.  in  HC1.     (Wein- 
land,  Z.  anorg.  1907,  64.  250.) 

Rubidium  thallic  sulphate,  RbTl(SO4)2. 
(MarshaU,  C.  C.  1902,  II.  1089.) 
-f  4H2O.     (Fortini,  Gazz.  ch.  it.  1905,  35. 

(2)  455.) 

Rubidium  thorium  sulphate,  Rb2SO4.  Th(S4O)2 

+2H2O. 

SI.  sol.  in  H2O.  (Manuelli,  Gazz.  ch.  it. 
1903,  32.  (2)  523.) 

Rubidium  titanium  sulphate,  Rb2SO4. 

Ti2(S04)3+24H20. 

Sol.  in  H2O  acidified  with  H2SO4.  De- 
comp. in  neutral  aq.  solution.  (Piccini,  Z. 
anorg.  189&,  17.  359.) 


26.  175.) 

Insol.  in  H2O. 

Insol.  in  H2SO4.  Decomp.  by  boiling  with 
cone.  H2SO4. 

Sol.  in  HC1.     (Stabler,  B.  1905,  38.  3980.) 

100  pts.  H2O  dissolve  2.56  pts.  salt  at  10°. 
Sp.  gr.  of  solution  at  4720°  =  1.915.  (Pic- 
cini, Z.  anorg.  1897,  13.  446.) 

Rubidium  zinc  sulphate,  Rb2SO4,  ZnS04+ 
6H2O. 

Sol.  in  H2O.  (Bunsen  and  Kopp,  Pogg. 
113.  337.) 

1  1.  H2O  dissolves  101  g.  anhydrous  salt 
at  25°.  (Locke,  Am.  Ch.  J.  1902,  27.  459.) 

Rubidium  zirconium  sulphate,  Zr2O3, 


sol. 


H2O. 


Ppt.    (Rosenheim,  B.  1905,  38.  815.) 

Ruthenic  sulphate,  Ru(S04)2. 
Deliquescent,    and    easily 
(Glaus,  A.  69.  246.) 

Samarium  sulphate,  basic,  (SmO)2SO4. 

Insol.  in  H2O  and  in  cold  dil.  H2SO4. 
(Matignon,  C.  R.  1905,  141.  1231.) 

Samarium  sulphate,  Sm2(SO4)3+8H20. 

Difficultly  sol.  hi  H2O. 

Much  less  sol.  than  Di2(SO4)3+8H2O. 
(Cleve.) 

2  05  pts.  anhydrous  salt  are  sol.  in  100  pts. 
H2O  at  25°.  (Keyes  and  James,  J.  Am. 
Chem.  Soc.  1914,  36.  635.) 

100  g.  Sm2(SO4)3+Aq  sat.  at  25°  contain 
3.426  g.  anhyd.  Sm2(SO4)3.  (Wirth,  Z.  anorg. 
1912,  76.  174.) 

Solubility  in  H2SO4+Aq  at  25°. 
n  =  equiv.  g.  of  H2SO4  in  1  1.  of  solvent. 
c  =  g  Sm2O3  in  100  g.  of  solution. 
ci  =  g.  Sm2(SO4)3  in  100  g.  of  solution. 


n 

C 

Cl 

n 

C 

Cl 

0 
0.1 
0.505 
1.1 

2.029 
2.038 
1.985 
1.821 

3.426 
3.441 
3.352 
3.075 

2.16 
6.175 
12.6 

1.43 
0.416 
0.0656 

2.416 
0.7025 
0.1107 

(Wirth,  Z.  anorg.  1912,  76.  174.) 

1012 


SULPHATE,  SAMARIUM  HYDROGEN 


Solubility  in  (NH4)2S(X»+Aq  at  25°. 

Samarium  sodium  sulphate,  Sm2(SO4)3, 

CO 

.»  • 

SI.  sol.  in  sat.  Na2SO4+Aq.     (Cleve,  Bull. 

$£.  ft 

Soc.  (2)  43.  166.) 

1§3 

-a 

Solid  phase 

2Sm2(SO4)3,  3Na2SO4+6H2O.    Only  double 

08**  i** 

§  as 

salt  formed  at  25°.     (Keyes  and  James,  J. 

&* 

-a 

Am.  Chem.  Soc.  1914,  36.  365.) 

2.1 

0.3 

Scandium  sulphate,  basic,  Sc2O(SO4)2. 

2.0 

0.8 

Sm2(SO4)3 

(Crookes,  Roy.  Soc.  Proc.  1908,  80.  A,  518.) 

2.8 
1.5 

1.1 
1.9 

Scandium  sulphate,  Sc2(S04)8. 

1.2 

2.7 

Anhydrous.    Easily  sol.  in  H2O. 

0.8 

7.4 

+2H20. 

0.8 

9.5 

+5H2O;  54.61  g.  of  pentahydrate  are  sol. 

0.8 

8.7 

in  100  cc.  H2O  at  25°.    (Wirth,  Z.  anorg.  1914, 

0.8 
0.8 
0  8 

18.8 
12.2 
12.3 

Sm2(SO4)3,  (NH4)2SO4,  7H2O 

87.  10.) 
Solubility  in  H2SO4+Aq  at  25°. 

0'.9 
1.0 

32.5 
46.3 

wan,.  4-  An                            g.  Sc2(SO4)sin 
100  g.  of  the  solution 

0.9 
1.3 

40.3 

77.5 

0.00                                28.52 

02 

0.5-n                              29.29 

Q.3 

77'.3 

(NH4)2S04 

1.0-n                               19.87 

0:6 

76.8 

4.86-n                              8.363 

9.73-n                               1.315 

(Keyes  and  James,  J.  Am.  Chem.  Soc.  1914, 
36.  637.) 

In    22.35-n    H2SO4    the    solid    phase    is 
Sc2(SO4)3,  3H2SO4  and  100  g.  sat.  solution 

Solubility  in  Na2SO4+Aq  at  25°. 

contain  0.484  g.  Sc2(S04)3. 

• 

(Wirth,  Z.  anorg.  1914,  87.  10.) 

81 

O-S 

+6H2O.     Extremely  sol.  in  H2O,  but  not 

|g<3 

!§§ 

Solid  phase 

deliquescent. 

«7! 

OQ 

Scandium  hydrogen     sulphate,   Sc2(SO4)3+ 

£a 

5  a 

CM 

3H2O. 

(Wirth.) 

0.1 
0.5 
1.9 

6.44 

2.0 
0.11 
0.03 
0.016 

Sm2(S04)3 

2Sm2(SO4)3,  3Na2SO4+6H20 
it 

Scandium      sodium      sulphate,      Sc2(SO4)8, 
3Na2SO4+12H2O. 
Sol.  inH2O.    (Cleve.) 

7  00 

0  008 

tt 

+  10H2O.     Sol.  in  H2O  and  in  excess  of 

4    .  V/U 

9.02 

0'.016 

it 

Na2SO4+Aq.     (Mevers,  Z.  anorg.  1914,  86. 

10.51 

0.012 

it 

279.) 

11.48 
13.58 

0.012 
0.010 

Silver    (argentoargentic)    sulphate,   Ag4S04, 
Ag2SO4+H2O. 

14.71 

0.010 

Gradually*  sol.  in  cone.,  but  not  attacked 

14.47 

0.009 

by  dil.,  HNO3+Aq.     Not  attacked  by  hot 

20.02 

0.012 

cone.  H2SO4.     (Lea,  Sill.  Am.  J.  144.  322.) 

23  42 

0.012 

, 

23^68 

o!ois 

Silver  sulphate,  Ag2SO4. 

25.93 

0.015 

it 

Sol.  in  200  pts.  cold,  and  less  than  100  pts.  boiling 

27.40 

0.011 

u    t 

H2O.      (Wittstein.) 
Sol.  in  88  pts.  boiling  H2O   (Schnaubart)  ;  in  87.25 

These  results  seem  to  indicate  that  there  is 
only  one  double  salt  formed  by  the  union  of 
Sm2(SO4)3  with  Na2SO4.  Formula  of  this 
salt  is  2Sm2(SO4)3,  3Na2SO4,  6H2O. 
(Keyes  and  James,  J.  Am.  Chem.  Soc.  1914, 
36.  635.) 

Samarium  hydrogen  sulphate,  Sm(HSO4)3. 

SI.  sol.  in  H2O.     (Matignon,  C.  R.  1905, 
141.  1230.) 

Ppt.    (Brauner,  Z.  anorg.  1904,  38.  331.) 


(Kremers) . 

100  pts.  H2O  at  15.5°  dissolve  1.15  pts.  Ag2SO4. 
(lire's  Di  ct.) 

Sol.  in  160  pts.  H2O  at  18.75°.    (Abl.) 

1 1.  H2O  dissolves  2.57  X 10  -2  g.-mol.  Ag2SO4 
at  25°.  (Drucker,  Z.  anorg.  1901,  28.  362.) 

1  1.  H2O  dissolves  7.707  g.  Ag2SO4  at  17°. 
(Euler,  Z.  phys.  Ch.  1904,  49.  314.) 

1  1.  H2O  dissolves  0.0267  mol.  Ag2SO4  at 
25°.  (Rothmund,  Z.  phys.  Ch.  1909,  69.  539.) 

1  1.  H2O  dissolves  8.35  g.  Ag2SO4  at  25°. 


SULPHATE,  SILVER 


1013 


(Hill  and  Simmons,  Z.  phys.  Ch.  1909,  67- 
603.) 

1  1.  H2O  dissolves  8.344  g.  Ag2SO4  at  25°. 
Sp.  gr.  of  solution  =  1.0052.  (Harkins,  J. 
Am.  Chem.  Soc.  1911,  33.  1812.) 

Solubility  in  H2O  at  t°. 


100. pts.  H20  dissolve  0.58  pt.  at  18°.  100 
ptsr  (NH4)2SO4+Aq  (15%)  dissolve  0.85  pt. 
Ag2SO4  at  18°.  Other  sulphates  have  little 
effect.  (Eder,  J.  pr.  (2)  17.  44.) 

Determinations  of  the  solubility  of  Ag2SO4 
in  (NH4)2SO4  at  temp,  between  16.5°  and  100° 


to                         Pts.  Ag2SO4  in  100  pts.  of 
the  solution. 

two  sulphates.     (Etard,  A.  ch.  1911,  (8)  24. 
221.) 

Solubility  of  Ag2SO4  in  (NH4)2SO4+Aq. 
G.  per  100  g.  H2O. 

14.5                             0.730 
33                                0.909 
51.5                              1.062 
75                                 1.237 
100                                 1.393 

(Barre,  A.  ch.  1911,  (8)  24.  211.) 

More  sol.  in  H2SO4+Aq  than  in  pure  H2O. 
Still  more  sol.  in  HNOs+Aq  and  still  more  in 
cone.  H2SO4,  from  which  it  is  pptd.  by  H2O. 
(Schnaubart.) 

Solubility  in  H2SO4+Aq  at  25°. 

(NH4)2S04 

Ag2S04 

(NH4)2SO4 

AgSO4 

Temp.  =33° 

Tamp.  =51° 

8.85 
15.90 
22.22 
27.25 
30.80 
35.88 
39.46 
43.22 

1.101 
1.331 
1.500 
1.585 
1.619 
1.627 
1.600 
1.557 

8.90 
16.27 
22.43 
32.10 
35.38 
39.03 
42.37 
45.05 

1.362 
1.680 
1.887 
2.061 
2.095 
2.082 
2.055 
2.026 

^H2SO4+Aq.                    Solubility  of  Ag2SO4 
Normality                            g.-mol.  per  litre 

0.02                           2.60X10-2 
0.04                          2.64X10-2 
0.10                          2.71  X  10  -2 
0.20                          2.75X10-2 

Temp.  =75° 

Temp.  =100° 

8.80 

15.23 
22.30 
28.25 
32.00 
35.82 
41.16 
46.46 

1.758 
2.155 
2.490 
2.734 
2.823 
2.889 
2.929 
2.902 

9.23 
15.00 
22.01 
27.00 
34.90 
38.70 
44.15 
47.63 

2.221 
2.626 
3.075 
3.325 
3.663 
3.772 
3.854 
3.867 

(Drucker,  Z.  anorg.  1901,  28.  362.) 

Solubility  of  Ag2SO4  in  acids  +Aq  at  25°. 
C  =  concentration  of  acid  in  acid+Aq  in 
milliequivalents  per  1. 
S  =  Solubility  of  Ag2SO4  in   acid+Aq  in 
milliequivalents  per  1. 

Acid 

C 

s 

HNO3 

0.0 
15.89 
31.78 
63.57 

53.98 
5.9.86 
65.32 
.75.90 

(Barre,  A.  ch.  1911,  (8)  24.  149,  202,  210.) 

Solubility  of  Ag2SO4  in  K2SO4+Aq. 
G.  per  100  g.  H2O. 

H2S04 

0.0 
29.02 
58.02 
105.26 

53.98 

54.88 
55.64 
56.82 

K.S04 

Ag>S04 

K2S04 

Ag»SO4 

Temp.  =33° 

Temp.  =51° 

(Swan,  J.  Am.  Uhem.  Soc.  1911,  33.  1814.) 
Solubility  in  HNO3+Aq  at  25°. 

3.22 
5.62 
8.37 
10.41 
11.80 

0.863 
0.940 
1.046 
1.117 
1.177 

3.20 
5.61 
8.40 
10.55 
13.16 
14.37 

1.023 
1.127 
1.247 
1.340 
1.450 
1.524 

Normality  HNOa 

Sp.  gr.  of  the 
solution 

g.  Ag2SO4 
dissolved  per  1. 

0.000 
1.0046 
2.0452 
4.017 
4.209 
5.564 
8.487 
10.034 

1.0054 
1.061 
1  .  1069 
1.1871 
1  .  1956 
1.2456 
1.3326 
1.3676 

8.350 
34.086 
49.010 
71.166 
73.212 
84.609 
94.671 
90.806 

Temp.  =75° 

Temp.  =100° 

3.12 
5.73 
8.43 
10.55 
13.17 
17.06 

1.273 
1.406 
1.554 
1.665 
1.806 
2.021 

3.23 
5.60 
8.45 
11.30 
15.07 
18.58 

1.488 
1.675 
1.890 
2.115 
2.410 
2.677 

(Hill  and  Simmons,  Z.  phys.  Ch.  1909,  67. 
603. 

Sol.  in  NH4OH,  and  (NH4)2CO3+Aq. 

(Barre,  A.  ch.  1911,  (8)  24.  149,  202,  210.) 

1014 


SULPHATE,  SILVER 


Solubility  in  K2SO4+Aq  at  25°. 

solubility  curves  for  various  temp,  all  end  at  a 
concentration  of  40%  Na2SO4,  that  is,  the 
mixed  crystals  formed  at  this  concentration 
are  equally  sol.  at  all  temp. 
(Barre,  C.  R.  1910,  160.  1323.) 

Solubility  in  Na2SO4+Aq  at  t°. 

^K2S04  +Aq                    Solubility  of  Ag2SCh 
Normality                            g.-mol.  per  litre 

0.02                            2.46X10-2 
0.04                            2.36  X10-2 
0.10                            2.31X10-2 
0.20                            2.32X10-2 

t° 

100  pts.  H2O  dissolve 

(Drucker,  Z.  anorg.  1901,  28.  362.) 

.  Solubility  in  Na2SO4+Aq  at  t°. 

Na2S04 

Ag2SO4 

18 

0.0 
0.25 
0.51 
•       0.74 
1.00 
1.48 
2.01 
2.50 
3.04 
4.00 
4.99 
10.10 
13.04 

0.766 
0.712 
0.682 
0.675 
0.665 
0.670 
0.673 
0.689 
0.703 
0.736 
0.768 
0.932 
1.028 

-  ±° 

AgzSCh  in 
100  pts:  H2O 

Na2SO4  in 
100  pts.  H2O 

14.5 

0.741 
0.904 
1.003 

5.278 
10.103 
13.045 

33 

0.972 
1.150 
1.320 
1.448 
1.548 
1.570 
1.549 
1.462 
1.199 
0.932 

5.345 
10.056 
15.185 
20.093 
25.412 
29.556 
34.732 
39.447 
44.693 
46.976 

33 

0.0 
0.25 
0.51 
0.75 
0.98 
1.50 
2.01 
2.48 
3.00 

0.917 
0.861 
0.835 
0.825 
0.816 
0.820 
0.832 
0.849 
0.867 

51 

.1.173 
:1.377 
1.572 
1.705 
1.787 
1.302 
„..„,.  t.,^27  
1.540 
1.188 
0.882 

5.407 
10.116 
15.146 
20.247 
25.196 
29.230  • 
34;£25 
39.302 
42.914 
44.464 

51 

0.00 
0.25 
0.49 
0.68 
1.02 
1.51 
1.90 
2.46 
2.92 
3.95 

1.081 
1.032 
1.010 
0.000 
0.995 
1.002 
1.017 
.034 
.053 
.103 

75 

1.458 
1.697 
J..934 

5.368 
9.813 
.15,260 
19.978 
25.556 
29.662 
35.278 
38.944 
41.365 

—  -    -- 

2.075 
2.161 
2.138 
1.910 
1.603 
1.156 

75 

0.00 
0.20 
0.47 
0.80 
0.98 
1.52 
1.96 
2.50 
2.98 
4.08 

.267 
.215 

1^210 
1.222 
1.238 

1^494 

100 

1.651 
2.012 
2.312 
2.351 
2.260 
2.012 
1.687 
1.158 

5.336 
10.153 
15.532 
25.451 
29.714 
34.718 
38.635 
40.160 

100 

0.00 
0.50 
1.01 
1.44 
1.94 
3.02 

Up   to   33°,   the  solubility  of  Ag2SO4  in 
NajSCh+Aq  increases  with  the  concentration 
of  Na2SO4;  above  33°  the  solubility  of  Ag2SO4 
rises*  W  "&"  Maximum"  at  a  certain  concentra- 
tion of  NaSO4  .dependent  on  the  temp.    The 

(Barre,  A.  ch.  1911,  (8)  24.  215.) 

SULPHATE  ACETYLIDE,  SILVER 


1015 


Solubility  in  salts  +Aq  at  25°. 

C  =  concentration  of  salt  in  salt+Aq  in 
milliequivalents  per  1. 
di  =  sp.  gr.  25°/4°  of  salt+Aq. 
S  =  solubility  of  Ag2SO4  in  salt+Aq  ex- 
pressed in  milliequivalents  per  1. 
d2  =  sp.  gr.  25°/4°  of  Ag2SO4+salt+Aq. 

Solubility  in  organic  compds.  +Aq  at  25°. 

Solvent 

Mol.  Ag2SO4  sol.  in 
1  litre 

Water 
0.5-N  Methyl  alcohol 
Ethyl  alcohol 
Propyl  alcohol 
Tert.  amyl  alcohol 
Acetone 
Ether 
Formaldehyde 
Glycol 
Glycerine 
Mannitol 
Glucose 
Sucrose 
Urea 
Dimethylpyrone 
Urethane 
Form  amide 
Acetamide 
Acetonitrile 
Glycocoll 
Acetic  acid 
Phenol 
Chloral 
Methylal 
Methyl  acetate 

0.0267 
0.0249 
0.0228 
0.0218 
0.0204 
0.0220 
0.0206 
0.0227 
0.0259 
0.0263 
0.0297 
0.0283 
0.0270 
0.0303 
0.0216 
0.0227 
0.0270 
0.0253 
0.0525 
0.0433 
0.0252 
0.0379 
0.0233 
0.0205 
0.0212 

Salt 

C 

di 

S 

d2 

none 

53.52 

KNO3 

24.914 
49.774 
99.870 

0.9986 
1.0002 
1.0034 

57.70 
61.13 
67.93 

1.0072 
1.0092 
1.0034 

Mg(N03)2 

24.764 
49.595 
99.460 

0.9985 
0.9999 
1.0026 

59.44 
64.32 
72.70 

1.0073 
1.0094 
1.0133 

AgN03 

24.961 
49.86 
99.61 

1.0007 
1.0044 
1.0112 

39.09 
28.45 
16.96 

1.0065 
1.0084 
1.0137 

K2S04 

25.024 
50.044 
100.0 
200.03 

0.9989 
1.0006 
1.0041 
1.0110 

50.66 
49.35 
48.04 
48.30 

1.0064 
1.0079 
1.0112 
1.0180 

MgS04 

20.22 
50.069 
100.04 
200.05 

0.9984 
1.0002 
1.0032 
1.0092 

52.21 
50.93 
49.95 
49.60 

1.0061 
1.0079 
1.0105 
1.0164 

(Rothmund,  Z.  phys.  Ch.  1909,  69.  539.) 

Insol.  in  methyl  acetate  (Bezold,  Dissert. 
1906;     Naumann,     B.     1909,     42.     3790); 
ethyl  acetate.    (Naumann,  B.  1904,  37.  3601)  ; 
liquid  methylamine.  (Franklin,  J.  Am.  Chem. 
Soc.    1906,  28.  1420);   acetone.     (Naumann, 
B.  1904,  37.  4329;  Eidmann,  C.  C.  1899,  II. 
1014.) 
Very  sol.  in  a  hot  mixture  of  H2SO4  and 
monobrombenzene,  less  sol.  in  cold.    (Couper, 
A.  ch.  (3)  62.  311.) 

(Harkins,  J.  Am.  Chem.  Soc.  1911,  33.  1813.) 

Solubility  of  Ag2SO4  in  salts  +Aq  at  25°. 

C  =  concentration   of  salt  in  salt+Aq  in 
milliequivalents  per  1. 
S  =  solubility    of   Ag2SO4    in    salt+Aq   in 
milliequivalents  per  1. 

Salt 

C 

S 

KHSO4 

0.0 
52.64 
105.26 

53.98 
52.18 
51.76 

K2S04 

0.0 
27.18 
54.34 

53.98 
50.90 
49.30 

(Swan,  J.  Am.  Chem.  Soc.  1911,  33.  1814.) 


Decomp.  by  alkali  thiosulphates+Aq. 
(Herschell.) 

100  ccm.  Ag2SO4+AgC2H3O2+Aq  sat.  at 
17°  contain  3.95  g.  Ag2SO4  and  8.30  g. 
AgC2H302  and  solution  has  sp.  gr.  =  1.0094. 
(Euler,  C.  C.  1904,  I.  1316.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898  20.  829.) 


Decomp.  by  H2O;  sol.  in  H2SO4.  (Stas.) 
Ag20,  3H20,  4S03+2H20=AgH3(S04)2+ 

H20.  As  above.  (Schultz,  Pogg.  133.  137.) 
2Ag2O,  3H2O,  5SO3+2H2O=Ag4H6(SO4)6 

+2H2O.    As  above.    (Schultz.) 

Silver  pyrosulphate,  Ag2S2C>7. 

Decomp.  by  H2O.     (Weber,  B.  17.  2497.) 

SUver  thallic  sulphate,  AgTl(SO4)j. 
(Lepsius,  Chem.  Ztg.  1890.  1327.) 

Saver  tin  (stannic)  sulphate,  Ag2Sn(SO4)«-f 
3H20. 

Ppt.     Decomp.    by  H2O.     Sol.    in    HC1. 
(Weinland,  Z.  anorg.  1907,  64.  250.) 

Silver  sulphate  acetylide,  Ag2S04,  2Ag2C2. 
(Plimpton,  Proc.  Chem.  Soc.  1892,  8.  109.) 


1016 


SULPHATE  AMMONIA,  SILVER 


Silver  sulphate  ammonia,  Ag2SO4,  2NH8. 

Completely  sol.  in  H2O.  (Rose,  Pogg.  20. 
153.) 

Ag2SO4,  4NH8.  Easily  sol.  in  HjO  or 
NH4OH+Aq  without  docomp.  (Mitschor- 
lich.) 

Silver  sulphate  mercuric  oxide,  Ag2SO4,  HgO. 
Insol.  in  HjO,  but  decomp.  even  in  the  cold. 
Sol.  in  JINOa  and  JI2H<)4.      (Find,  (J;i//.  <-h. 
it.  1911,  41.  (2)  548.) 

Silver  sulphate  sulphide,  Ag>S04,  Ag2S. 

Decomp.  by  hot  H2O  or  cold  HCl+Aq. 
Sol.  in  boiling  HNO8+Aq.  (Poleck  and 
Thttmmel,  B.  18.  2435.)  <i-H 

Sodium  sulphate,  Na2SO4. 

Anhydrous. 

1  pt.  NaiSO4  is  sol.  in  7.367  pts.  HjO  at  15°  (Gerlach) ; 
in  8.52  pts.  HjO  at  '13.3°  (Poggendorf) ;  in  10  pts.  H2O 
at  13°,  and  in  3.3  pts.  H»O  at  62.2°  (Wenzel). 

100  pts.  H2O  at  0°  dissolve  5.155  pts.  Na»SO4(Pfaff, 
A.  99.  226);  at  100.6°  dissolve  45.985  pts.  Nl.-.-sn. 
(Griffiths). 

See  below  for  further  data. 

+7HtO.    Efflorescent.    Insol.  in  alcohol. 

See  below  for  further  data. 

+10H»O. 

Na2SO4  +  10H2O  is  sol.  in  H2O  with  absorp- 
tion of  heat;  20  pts.  Na2SO4+10H2O  mixed 
with  100  pts.  H2O  at  12.5°  lower  the  tempera- 
ture 6.8°.  (Rudorff,  B.  2.  68.) 

Sol.  in  2.33  pts.  H»O  at  19°,  or  100  pts.  HiO  at  19° 
dissolve  42.8  pts.  NaiSCU+lOHjO.  (Schiff,  A.  109. 
326.) 

100  pts.  HsO  dissolve  a  pts.  \.-.-st  >,  and  b  pts.  \ :.  -s»  > .. 
+10HiO  at  t°. 


t° 

a 

b 

t° 

a 

b 

0 

5.02 

12.17 

33.88 

50.04 

312.11 

11.  C.7 

10.12 

26.38 

•10.  If, 

•1S.7S 

291.44 

i.r«o 

11.74 

:u.:u 

45.04 

47.81 

276.91 

17.91 

16.73 

IS.  US 

50.40 

4(5  !  82 

262  .  35 

2r>.or, 

2S  .  1  1 

'.»'.)  -IS 

59.79 

45.42 

2X.7l» 

37.35 

161.53 

70.61 

44.35 

30.75 

4S  05 

215.77 

84.42 

42.96 

:u.H4 

47.37 

270.22 

103.17 

42.65 

:«  7:1 

50.65 

322.12 

(Gay-Lussac,  A.  ch.  (2)  11.  312.) 

Maximum  solubility  is  at  33°  from  experiment  and 
theoretical  considerations.  At  this  temp.  NatSO4  + 
lOHiO  is  converted  into  NaiSCh.  (Kopp,  A.  34.  271.) 


100  pts.  H-..0  at  t.°  dissolve  pts.  Na,SO<  f  IOH.-0. 


if 

Pts. 
Na2S04 

t° 

Pts. 
Na2SO4 

0 
17.9 

4.53 
16.28 

24.1 
33 

25.92 
50.81 

t° 

Pts. 
NinSO* 
-flOHiO 

t° 

Pts. 
Massif 
-r-lOH-t) 

t° 

Pts. 
NatSO4 
-HlOHjO 

2.5 
7.5 

1-2  .f> 

is.rr, 

LT. 
31.25 

11.39 
ic.  ;is 
iM»  .  o;< 
:o  .  rs 
L48.88 
170.  W 

37.50 

4:1   7  r. 
60 

at;   IT. 
•  51!   a 

<>s  .  :;> 

L>'.M   01 
•2ti\   IH 

i>s;,.of, 

IMS   11 
2  J'J  2-2 
242.SS 

75 
81.25 
87.50 

'.u  ::> 

100 

241.68 
217.20 
220.65 
225!  40 
241.69 

(Brandes  and  Firnhabor.  1884.) 

1  pt.  NjSO«+10H2O  is  sol.  in  6.1  pts.  H2O  at  7.5°; 
3.44  pts.  at  12.5°;  2.41  pts.  at  18.75°;  and  1.724  pts. 
at  .20°.  (Karsten.) 

1  pt.  NazSO4+10H2O  is  sol.  in  2.86  pts.  cold,  and 
0.8  pt.  boiling  HzO  (Bergmann) ;  in  3  pts.  cold,  and 
0.5  pt.  boiling  HzO  (Wittstein) ;  in  4  pta.  cold,  and  1  pt. 
boiling  H2O  (Fourcroy) ;  in  3  pts.  H2O  at  18.75°  (Abl). 

100  pts.  H2O  dissolve  12.494  pts.  Na2SO4  or  35.492 
pts.  Na2SO4-|-10H2O  at  15°,  and  sp.  gr.  of  solution  = 
1.10847- (Michel  and  Krafft,  A.  ch.  (3)  41.  478.) 

100  pts.  H2O  dissolve  39.4  pts.  cryst.  salt  at  15.5°; 
80  pts.  cryst  salt  at  100°.  (lire's  Diet.) 

100  pts.  H2O  dissolve  pts.  Na2SO4  at  t°. 


(Diacon,  J.  B.  1866.  61.) 

Solubility  of  Na2SO4  in  H2O  at  various  pres- 
sures and  temp.  Pts.  Na2SO4  contained 
in  100  pts.  sat.  Na2SO4-f-Aq  at  A  pressure 
in  atmos.  and  t°  are  given. 


A 

1 
20 

0° 

15° 

15.4° 

A 

15° 

4.40 
4.53 

11.32 
10.78 

11.4 
10.74 

30 
40 

10.05 
10.33 

(Mailer,  Pogg.  117.  386.) 

The  solubility  of  Na2SO4+10H2O  increases 
with  the  temperature  from  0  to  34°.  At  34° 
and  above,  it  is  converted  into  the  anhydrous 
salt,  the  solubility  of  which  is  least  at  103.17°, 
which  is  the  boiling  point  of  the  saturated 
solution,  and  increases  by  cooling  from  that 
temp,  down  to  18-17°.  Below  the  latter 
temperature  the  anhydrous  salt  cannot  exist 
in  the  presence  of  H2O,  but  is  converted  into 
Na2SO4-f7H2O,  or  Na2SO4+10H2O.  The 
solubility  of  Na2SO4+7H2O  increases  with 
the  temperature  from  0-26°,  and  at  27°  it  is 
converted  into  the  anhydrous  salt. 

Thus  there  are  two  different  rates  of  solu- 
bility for  Na2SO4  for  temperatures  from 
0-18°,  three  different  rates  from  18-26°,  two 
from  26-34°,  and  only  one  above  34°. 

1.  By  heating  Na2SO4+10H2O  to  fusion 
and  raising  the  heat  until  the  liquid  boils, 
placing  in  a  closed  vessel  and  cooling,  the 
greater  part  of  the  anhydrous  salt,  which 
separates  out  on  heating,  redissolves  on  cool- 
ing, and  the  amount  increases  as  the  temp, 
falls  until  18°  is  reached.  Below  18°  Na2SO< 
+7H2O  is  formed.  Saturated  Na2SO4+Aq 
thus  obtained  contains  for  100  pts.  HO  at: 

18°        20°       25°       26° 
53.25    52.76    51.53    51.31  pts.  Na2S04, 

30°       33°       34°       36° 
50.37    49.71    49.53    49.27  pts.  Na2SO4.    j 

>  2.  By  allowing  the  boiling  saturated  solu 
tion  free  from  undissolved  salt  to  cool  to  0 


SULPHATE,  SODIUM 


1017 


with  exclusion  of  air  until  crystals  of  Na2SO4 
+7H2O  are  formed,  then  removing  the 
greater  part  of  the  mother  liquor  with  a  warm 
pipette,  and  warming  the  rest  of  the  mother 
liquor  with  the  excess  of  crystals,  the  crystals 
dissolve  in  increasing  quantity  between  0°  and 
26-27°,  so  that  at  27°  the  solution  contains 
56  pts.  Na2SO4  to  100  pts.  H2O.  The  remain- 
ing undissolved  crystals  of  Na2SO4+7H2O  be- 
gin to  melt  very  slowly  at  27°,  more  quickly 
at  higher  temperatures,  and  cause  the  separa- 
tion of  anhydrous  crusts,  and  thus  the 
strength  of  the  solution  is  gradually  lowered 
to  the  normal.  Saturated  solutions  prepared 
in  this  way  contain  for  100  pts.  H2O  at: 


13° 

34.27  pts.  Na2SO4, 
92.9  pts.  Na2S04+7H2O. 

17° 

39.99  pts.  Na2SO4, 
111.0  pts.  Na2SO4  +7H2O, 

20° 

44.73  pts.  Na2SO4, 
140.0  pts.  Na2SO4+7H20, 


202.6  pts.  Na2SO4+7H2O. 

3.  Solutions  obtained  by  shaking  H20  with 
Na2SO4+10H2O  contain  for  100  pts.  H2O  at 


0° 

10° 

19.62 

30.49 

or  44.89 

78.9 

15° 

16° 

37.43 

38.73 

or  105.8 

117.4 

18° 

19° 

41.63 

43.35 

or  124.6 

133.0 

25° 

26° 

52.94 

54.97 

or  188.5 

202.6 

0° 
5.02 
or  12.16 

18° 
16.80 
or  48.41 

26° 
30.00 
or  109.81 

33° 
50.76 
or  323.1 


10° 
9.00 
23.04 

20° 
19.40 

5S.S5 


15° 

13.20  pts.  Na2SO4, 
35.96  pts. 

25° 

28.00  pts.  Na2SO4, 
98.48  pts.  Na2SO4H-10H2O 

30° 

40.00  pts.  Na2SO4, 

184.1  pts.  Naz 

34° 
55.0  pts.  Na2SO4. 

412.2  pts.  NazSO.+lOHjO. 


35° 
0.2 

40° 

48.8 

45° 

47.7 

50° 
46.7 

55° 
45.9  pts. 

Na2S04, 

60° 
45.3 

65° 
44.8 

70° 
44.4 

75° 
44.0 

80° 
43.7  pts. 

Na2S04, 

85° 
43.3 

90° 
43.1 

95° 
42.8 

100° 
42.5 

103.5° 
42.2  pts. 

Na2S04. 

At  34°,  XajSO4+10H2O  begins  to  melt  in 
its  crystal  H2O.  As  long  as  there  is  a  con 
siderable  quantity  of  unchanged  crystals 
present,  the  solution  contains  55  pts.  Na2SO 
for  100  pts.  H2O,  but  as  the  hydrous  salt  de- 
creases in  amount  and  becomes  converted  into 
the  anhydrous  salt,  the  solution  becomes 
weaker  and  contains  only  49.53  pts.  N 
for  100  pts.  HjO  after  warming  for  6  or  8  hours 
at  34°.  In  the  same  way  temporary  solutions 
can  be  obtained  at  36-40°  with  55-56  pts 
NajSO4  to  100  pts.  HjO,  but  this  amoun 
sinks  to  the  normal  even  more  quickly  than 
at  34° 

XajSO4  dehydrated  at  100-150°,  after  the 
addition  of  1J'*-1H  pts.  H^,  gives  a  solution 
between  0°  and  32°  of  the  same  strength  as 
NaiSO4-f  lOHjO,  but  at  34°  a  solution  with 


5  pts.  Na2SO4  to  100  pts.  H2O  cannot  be 
btained,  but  one  with  49.53  pts.  is  formed. 
Lowel,  A.  ch.  (3)  49.  32.) 

4.  Solubility  of  anhydrous  salt.    Above  34°, 
00  pts.  H2O  dissolve  at: 


(Mulder.) 
Solubility  in  100  pts.  H2O  at  t°. 


t° 

Pts. 

Na2SO4 

t° 

Pts. 

NH2SO4 

t° 

Pts. 
Na,SO« 

0 

4.8 

35 

50.2 

70 

44.4 

1 

5.1 

36 

49.9 

71 

44.3 

2 

5.4 

37 

49.6 

72 

44.2 

3 

5.7 

38 

49.3 

73 

44.2 

4 

6.0 

39 

49.1 

74 

44.1 

5 

6.4 

40 

48.8 

75 

44.0 

6 

6.8 

41 

48.5 

76 

44.0 

7 

7.3 

42 

48.3 

77 

43.9 

8 

7.8 

43 

48.1 

78 

43.8 

9 

8.4 

44 

47.9 

79 

43.7 

10 

9.0 

45 

47.7 

80 

43.7 

11 

9.7 

46 

47.5 

81 

43.6 

12 

10.5 

47 

47.3 

82 

43.5 

13 

11.4 

48 

47.1 

83 

43.5 

14 

12.4 

49 

46.9 

84 

43.4 

15 

13.4 

50 

46.7 

85 

43.3 

16 

14.5 

51 

46.6 

86 

43.3 

17 

15.7 

52 

46.4 

87 

43.2 

18 

16.9 

53 

46.2 

88 

43.2 

19 

18.2 

54 

46.1 

89 

43.1 

20 

19.5 

55 

45.9 

90 

43.1 

21 

20.9 

56 

45.8 

91 

43.0 

22 

22.5 

57 

45.7 

92 

43.0 

23 

24.1 

58 

45.6 

93 

42.9 

24 

25.9 

59 

45.4 

94 

42.9 

25 

27.9 

60 

45.3 

95 

42.8 

26 

30.1 

61 

45.2 

90 

42.7 

27 

32.4 

62 

45.1 

97 

42.6 

28 

35.0 

63 

45.0 

98 

42.6 

29 

37.8 

64 

44.9 

99 

42.5 

30 

40.9 

65 

44.8 

100 

42.5 

31 

44.2 

66 

44.7 

101 

42.4 

32 

47.8 

67 

44.6 

102 

42.3 

32.75 

50.65 

68 

44.5 

103 

42.2 

33 

50.6 

69 

44.5 

103.5 

42.2 

34 

50.4 

(Mulder,  Scheik.  Verhandel.  1864.  123.) 


100  pts.  dissolve  at: 
0°        34°        100° 
5     78.8(?)    42.7 


120° 
41  95  pts. 


140°        160° 

42.0      42.9 

(Tilden  and 


180°        230° 

44.25     46.4pte.Na£O«. 
Loud.  R.  Soc.  Proc. 


1018 


SULPHATE,  SODIUM 


Solubility  decreases  above  230°.     (Etard 
C.  R.  113.  854.) 

Sat.  Na2SO4+Aq  contains  at: 
0°       7°       13°     24°     28°     30° 
4.1      6.2      9.9     19.3    25.2    29.5%  Na2S04 

49°     62°     83°     99°     134°   150° 

32.8  31.3    30.0    29.7    29.4   29.8%  Na2S04 

190°   240°  279°   320° 

29.9  30.0    24.5    17.8%  Na2SO4. 

(Etard,  A.  ch.  1894,  (7)  2.  548.) 

Solubility  of  Na2SO4  in  H20  at  t°. 
G.  per  100  g.  H2O. 


t° 

Na2S04 

Sp.  gr. 

"t 

Na2S04 

Sp.  gr. 

0.70 

4.71 

.0432 

33.5 

49.39 

1.3307 

10.25 

9.21 

.0802 

38.15 

48.47 

1.3229 

15.65 

14.07 

.1150 

44.85 

47.49 

1.3136 

24.90 

27.67 

.2067 

60.10 

45.22 

1.2918 

27.65 

34.05 

.2459 

75.05 

43.59 

1.2728 

30.20 

41.78 

.2894 

89.85 

42.67 

1.2571 

31.95 

47.98 

.3230 

101.9* 

42.18 

1.2450 

*  B.-pt. 

(Berkeley,  Phil.  Trans.  Roy.  Soc.  1904,  203. 
A,  189.) 

Transition  point  from  Na2SO4+10H2O  to 
Na2SO4  =  32.5°  (Berkeley);  32.383°.  (Rich- 
ards and  Churchill,  Z.  phys.  Ch.  1899,  28. 
314.) 

100  g.  Na2SO4+Aq  sat.  at  15°  contain 
11.5  g.  anhydrous  Na2SO4;  21.9  g.  at  25°. 
(Schreinemakers,  Arch.  Ne'er.  Sc.  1910,  (2) 
16.  81.) 

1  1.  Na2SO4+Aq  sat.  at  25°  contains  1.881 
mols.  Na2SO4.  (Herz,  Z.  anorg.  1911,  70. 
127.) 

Solubility  in  H2O  at  t°. 


t° 

Mol.  %  Na2SO4 

Tl 

CO 

62 

5.39 

n* 

70 

5.27 

ar< 

72 

5.25 

h 

80 

5.18 

120 

5.04 

_5 

190 

5.25 

Nf 

192 

5.27 

as 

208 

5.39 

Ot 

241 

5.39 

10 

250 

5.04 

i 

279 

4.12 

Ch 

319 

2.56 

r} 
n 

252 

4.9 

ar 

310 

3.2 

, 

340 

1.8 

me 

365 

0.0 

id 

(Wuite,  Z.  phys.  Ch.  1913,  86.  364.) 

I* 

nc 

Supersaturated  solutions  of  NaSO4  are 
easily  formed;  when  Na2SO4+Aq  sat.  at  its 
b.-pt.  is  hermetically  sealed,  no  crystals  are 
deposited  on  cooling  (Lowel).  Supersat. 
Na2SO4+Aq  may  also  be  obtained  by  cooling 
hot  sat.  Na2SO4+Aq  in  flasks  loosely  stop- 
pered with  cotton  wool  (Schroeder,  A.  109. 
45),  or  by  covering  the  containing  vessel  with 
a  glass  plate,  watch-glass,  card,  etc.,  or  by 
covering  the  liquid  itself  with  a  layer  of  oil, 
and  then  allowing  to  cool. 

Hot  Na2S04+Aq  containing  1  pt.  H2O  to 
1  pt.  Na2SO4+10H2O  does  not  crystallise  on 
slowly  cooling  or  on  being  quickly  cooled  by 
immersion  in  cold  water,  if  it  is  contained 
in  a  barometer  tube  freed  from  air  by  boiling, 
or  in  an  exhausted  well-closed  vessel,  or  in  an 
open  vessel  with  a  layer  of  oil  of  turpentine 
on  it  (Gay-Lussac) ;  or  in  a  vessel  containing 
air,  either  well  stoppered  or  furnished  with  a 
loose  cover  (Schweigger) ;  or  in  an  open  vessel 
under  a  bell  jar  full  of  air  and  closed  at  the 
bottom  with  a  water  joint;  or  in  open  bottles 
placed  in  a  quiet  situation;  or  in  an  open 
glass  enclosed  in  a  stoppered  vessel,  contain- 
ing air  and  some  KOH  for  drying;  in  this  case 
Na2SO4+10H20  effloresces  from  the  solution, 
and  when  washed  down  again  does  not  cause 
instant  crystallisation,  but  redissolves. 

The  crystallisation  of  a  solution  cooled  in 
this  way  may  often  be  brought  about  in- 
stantaneously, or  often  again  after  a  short 
tune;  (1)  by  agitation,  when  the  solution  has 
been  cooled  in  an  open  vessel;  (2)  by  access 
of  air  caused  by  opening  the  vessel,  the  crys- 
tallisation taking  place  the  more  rapidly  the 
iarger  the  opening.  In  this  case  the  crystallis- 
ation begins  at  the  top,  where  the  solution,  the 
vessel  and  the  air  come  in  contact;  when  a 
eiOf  dust  falls  in  the  liquid  the  crystal- 
isation  begins  a  little  under  the  surface. 
When  the  solution  has  been  cooled  in  vacuo,  a 
Bubble  of  air,  hydrogen,  carbonic  acid,  or 
litrous  oxide  is  sufficient  to  set  up  the  crystal- 
isation;  (3)  by  contact  with  a  solid  body. 
The  latter  do  not  cause  crystallisation  when 
iooled  in  contact  with  the  liquid,  nor  (except- 
ng  a  crystal  of  Na2SO4+10H2O)  when  they 
are  moistened  or  warmed  before  contact  with 
he  solution. 

Supersat.      Na2S04-J-Aq    is    brought    to 
xystallisation  by  addition  of  a   crystal  of 
Sfa2SO4  +  10H2O,  or  an  isomorphous  substance 
is   Na2SeO4+10H2O,    or   Na2CrO4  +  10H2O. 
Other  crystals,  as  MgSO4+7H2O,  etc,,  have 
no  action.    (Thomfeon,  Chem.  Soc.  35.  199.) 
See  also  Hartley,  Jones  and  Hutchinson, 
ihem.  Soc.  1908,  93.  825,  on  "Spontaneous 
rystallisation  of  sodium  sulphate  solutions," 
and  de  Cpppet  (A.  ch.  1907,  (8)  10.  457)  on 
ame  subject. 

A  more  extended  discussion  of  the  pheno- 
mena and  causes  of  supersaturation  is  not  con- 
idered  to  the  within  the  scope  of  this  work. 

Na2SO4+Aq  sat.  at  15°  has  sp.  gr.  1.10847  (Michel 
nd  Krafft);  at  15°  has  sp.  gr.  1.119  (Stolba);  at  16° 


SULPHATE,  SODIUM 


1019 


has  sp.  gr.  1.1162  (Stolba) ;  at  10°  contains  29  pts. 
Na2SO4  to  100  pts.  HzO  (supersaturated?),  and  has 
sp.  gr.  1.1259  (Karsten). 

Sp.  gr.  of  Na2SO4+Aq  at  19.5°. 


% 

Na2SO4 

Sp.  gr. 

% 
Na2S04 

Sp.  gr. 

2.894 
5.589 
7.995 

1  .  0262 
1  .  0509 
1.0733 

10.538 
12.473 

1.0977 
1.1162 

(Kremers,  Pogg.  95.  120.) 
Sp.gr.  of  Na2SO4+Aq. 


+10H2O 

Sp.  gr. 

Na2SO4 
+10H2O 

Sp.  gr. 

1.262 

.005 

13.744 

1.055 

2.522 

.010 

14  .  975 

1.060 

3.780 

.015 

16.203 

1.065 

5.035 

.020 

17.426 

1.070 

6.288 

.025 

18.645 

1.075 

7.538 

.030 

19.860 

1.080 

8.786 

1.035 

21.071 

1.085 

10.030 

1.040 

22.277 

1.090 

11.272 

1.045 

23.478 

1.095 

12.510 

1.050 

24  .  674 

1.100 

(Schmidt,  Pogg.  132.  132.) 

Sp.  gr.  of  Na2SO4+Aq  at  19°. 


%  Na2SO4 
+10H20 

Sp.  gr. 

%  Na2SO4 
+10H2O| 

Sp.  gr. 

1 

1.0040 

16 

1.0642 

2 

1.0079 

17 

1.0683 

3 

1.0118 

18 

1.0725 

4 

1.0158 

19 

1.0766 

5 

1.0198 

20 

1.0807 

6 

.0232 

21 

1.0849 

7 

.0278 

22 

.0890 

8 

.0318 

23 

.0931 

9 

.0358 

24 

.0973 

10 

.0398 

25 

.1015 

11 

1.0439 

26 

.1057 

12 

1.0479 

27 

.1100 

13 

1.0520  • 

28 

.1142 

14 

1.0560 

•      29 

.1184 

15 

1.0601 

30 

.1226 

(Schiff,  A.  110.  70.) 
Sp.  gr.  of  Na2SO4+Aq  at  15°. 


% 

Sp.  gr. 
if 
Na2SO4 

Sp.  gr. 
if 
Na2S04 
+10H20 

% 

Sp.  gr. 

Naj8O< 

+10H2O 

% 

Sp.fgr. 

Na2SO4 
+10H2O 

1 

1.0091 

1.004 

11 

1.044 

21 

.086 

2 

1.0182 

1.008 

12 

1.047 

22 

.090 

3 

1.0274 

1.013 

13 

1.052 

23 

.094 

4 

1.0365 

1.016 

14 

1.056 

24 

.098 

5 

1.0457 

1.020 

15 

1.060 

25 

.103 

6 

1.0550, 

1.024 

16 

1.064 

26 

.107 

7 

1.0644 

1.028 

17 

1.069 

27 

1.111 

8 

1.0737 

1.032 

18 

1.073 

28 

1.116 

9 

1.0832 

1.036 

19 

1.077 

29 

1.120 

10 

1.0927 

1.040 

20 

1.082 

30 

1.125 

(Gerlach,  Z.  anal.  8.  287.) 


Sp.  gr.  of  Na2SO+Aq  at  24.8°.  a=no.  of 
g.,  equivalent  to  3^  mol.  wt.,  dissolved  in 
1000  g.  H2O;  b  =  sp.  gr.  if  a  is  Na2SO4+ 
10H2O,  3^  mol.  wt.  =  161;  c  =  sp.  gr.  if  a 
is  Na2SO4,  y>  mol.  wt.=71. 


1.054 
1.098 
1.134 


1.059 
1.114 
1.165 


1.163 
1.188 
1.209 


1.213 


(Favre^and  Valson,  C.  R.  79.  968.) 
Sp.  gr.  of  Na2SO4+Aq  at  18°. 


%  Na2SO4 


5 
10 


Sp.  gr. 


1.0450 
1.0915 


%  Na2S04 


15 


Sp.  gr. 


1 . 1426 


(Kohlrausch,  W.  Ann.  1879.  1.) 

Sp.  gr.  of  Na2SO4+Aq  at  20°  containing 
0.5  mol.  Na2SO4  to  100  mols.  H2O  =  1.03466; 
1.0  mol.  Na2SO4  to  100  mols.  H2O  =  1.06744. 
(Nicol,  Phil.  Mag.  (5)  16.  122.) 

Sp.  gr.  of  Na2SO4+Aq  at  25°. 


Concentration  of  Na2SO4 
+Aq 

Sp.jsr. 

1-normal 

Vr-      " 

V«-     " 

Vs         " 

1.0606 
1.0309 
1.0156 
1.0079 

(Wagner,  Z.  phys.  Ch.  1890,  6.  39.) 

Sp.  gr.  at  16°/4°  of  Na2SO4+Aq  containing 
9.4043%  Na2SO4  =  1.08655.  (Schonrock,  Z. 
phys.  Ch.  1893,  11.  781.) 

Na2SO4+Aq  containing  25.51%  Na2SO4 
has  sp.  gr.  20°/20°  =  1.2527.  Na2SO4+Aq 
containing  10.14%  Na2SO4  has  sp.  gr.  20°/20° 
=  1.0938.  (Le  Blanc  and  Rohland,  Z.  phys. 
Ch.  1896,  19.  278.) 

Sp.  gr.  of  Na2SO4+Aq  at  f.7.5°,  when  p  = 
per  cent  strength  of  solution;  d  =  ob- 
served density;  and  w  =  volume  cone,  in 


grs.  percc.  (TT^  = 


p. 

d. 

w. 

13.06 

.1226 

0.14662 

11.75 

.  1094 

0.13043 

10.68 

.0990 

0.11737 

8.544 

.0784 

0.09214 

6.762 

.0615 

0.07178 

4.015 

.0358 

0.04159 

2.599 

.0225 

0.02658 

2.375 

.0204 

0.02423 

1.818 

.0154 

0.01846 

1.349 

1.0109 

0.01364 

0.5204 

1  .0037 

0.00522 

0.2921 

1.0014 

0.00293 

(Barnes,  J.  phys.  Chem.  1898,  2.  543.) 


1020 


SULPHATE,  SODIUM 


Sp.  gr.  of  Na2SO4+Aq  at  20°. 

B.-pt.  of  Na2SO4+Aq  containing  pts.  Na2SO4 
to  100  pts.  H2O. 

Normality  of 
Na2SO4+Aq 

%  Na2S04 

Sp.  gr. 

B.-pt. 

Pts.  Na2SO4 

B.-pt. 

Pts.  Na2S04 

0.97 
0.48 

12.36 
6.41 

1.1138 
1.0570 

100.5° 
101.0 
101.5 
102.0 

9.5 
18.0 
26.0 
33.0 

102.5° 
103.0 
103.2 

39.0 
44.5 
46.7 

(Forchheimer,  Z.  phys.  Ch.  1900,  34.  23.) 

Sp.  gr.  of  sat.  Na2SO4,  10H2O+Aq  at  t°. 


t° 

wt.  of  1  ccm.  of 
the  solution 

100  g.  H2O 
dissolve  g. 
Na2SO4+10H20 

0 

.040 

12.16 

5 

.058 

10 

.078 

2i!o4 

15 

.109 

35.96 

18 

.137 

48.41 

20 

.156 

58.35 

25 

.209 

98.48 

26 

.222 

109.81 

30 

.287 

184.1 

33 

.312 

323.1 

34 

.317 

413.2 

35 

.317 

(Tschernaj,  J.  Russ.  Phys.  Chem.  Soc.  1914, 
46.  8.) 


Sp.  gr.  and  b.-pt.  of  Na2SO4+Aq.  Na2SO4-r-Aq 
containing  P  pts.  Na2SO4-flOH2O  for  every  100  pts. 
H2O  has  given  sp.  gr.  and  b.pt. 


P 

Sp.  gr. 

B.-pt. 

P 

Sp.  gr. 

B.-pt. 

1 

1.005 

100.5° 

16 

1.064 

101.25° 

2 

1.008 

100.62 

17 

.067 

101.25 

3 

1.014 

100.62 

18 

.070 

101.37 

4 

1.020 

100.75 

19 

.072 

101.37 

5 

1.021 

100  .  75 

20 

.074 

101.37 

6 

1.028 

100.87 

21 

.076 

101.37 

7 

1.030 

100.87 

22 

.078 

101.5 

8 

1.032 

101.0 

23 

.080 

101.5 

9 

1.036 

101.0 

24 

.082 

101.5 

10 

1.040 

101.0 

25 

.084 

101.5 

11 

1.043 

101.12 

26 

.090 

101.5 

12 

1.050 

101.12 

27 

.092 

101.63 

13 

1.055 

101.25 

28 

1.095 

101.63 

14 

1.060 

101.25 

29 

1.098 

101.63 

15 

1.062 

101.25 

30 

1.100 

101.75 

(Brandes  and  Gruner,  1827.) 


Saturated  solution  boils  at  103.17°  (L6wel), 
103.5°  (Mulder),  105°  (Kremers),  100.5° 
(Griffiths),  100.8°  (Gerlach). 

Crust  forms  at  102.9°;  highest  temp.,  103.2°, 
and  solution  contains  43.9  pts.  Na2SO4  to  100 
pts.  H2O.  (Gerlach,  Z.  anal.  26.  426.) 


(Gerlach,  Z.  anal.  26.  430.) 


M.-pt.  of  Na2SO4+10H2O=34°.     (Tilden, 
Chem.  Soc.  45.  409.) 
Sol.  with  decomp.  in  HCl+Aq. 

Solubility  in  H2SO4+Aq  at  25°. 

1000  g.  of  the 
solution  contain 

Solid  phase 

Mols 
H2S04 

Mols 
Na2S04 

0.286 

0.338 
0.884 
1.576 
1.666 
2.611 

1.539 
1.671 
1.742 
2.256 
2.363 
2.437 
2.091 

Na2S04,  10H20 

a 

Na2SO4,  10H2O+Na2SO4 

Na2SO4+Na3H(SO4)2 

(( 

Na3H(SO4)2+Na3H(SO4)2,  H2O 

(D'Ans,  Z.  anorg.  1906,  49.  356.) 


Solubility  of  Na2SO4  in  H2SO4+Aq  at  25. c 


1000  g.  of  the  solution 
contain 

Solid  phase 

Mol.  Na2S04 

Mol.  H2SO4 

1.55 

0.08 

Na2SO4 

1.59 

0.147 

(C 

1.85 

0.60 

Na2SO4,  10H2O 

2.00 

0.763 

" 

0.77 

4.23 

NaHSO4.  H2O 

0.47 

4.96 

« 

0.32 

6.61 

Na2HSO4 

0.305 

6.87 

u 

0.07 

7.18 

Na3H(S04)2 

0.79 

8.78 

(D'Ans,  Z.  anorg.  1909,  61.  92.) 


10  ccm.  of  sat.  Na2SO4+ absolute  H2S04 
contain  approx.  2.999  g.  Na2SO4.  (Bergius, 
Z.  phys.  Ch.  1910,  72.  355.) 


SULPHATE,  SODIUM 


1021 


Solubility  in  H2SO4+Aq  at  25°. 
Solid  Phase,  Na2SO4-(-10H2O. 

Solubility  in  NaOH+Aq  at  25°. 

1000  g.  of  the 
solution  contair 

i 

Solid  phase 

4 

Millimols  H2SO4 
in  10  ccm. 

Millimols  Na2S04 
in  10  ccm. 

Mols         Mols 
(NaOH)'j    Na2SC 

18.81 

0             1.54               Na2SO4,  10H2O 

5.W 

22.38 

0.074      1.41                            " 

7.79 

24.65 

0.70       1.08 

1   47        0  QO        NfloSO,,    lOHoO-J-NfloSfh 

(Herz,  Z.  anorg 

1912,  73.  276.) 

J.  .  TZ  f             U  .  t/U            .ii  d>2fc3Vy4}    Av/Xi2^-'    |^-^  ct2^vy4 

2.02       0.59                     Na2SO4 
2.82       0.24 

3.52       0.126                          " 

5.83       0.013                          " 

Solubility  in  H2SO4+Aq  at  25°. 

6.62         ...                  NaOH,  H2O 

1000  g.  of  the 

Solid  phase 

(D'Ans  and.Schreiner,  Z.  anorg.  1910,  67.  437.) 

solution  contain 

Sol.  in  sat.  NH4Cl+Aq. 

T"fc            "11                     11_             Jj.1                  1'                  j.       TT'/^ll      I 

Mols 
SO3 

Mols 
Na2S04 

Rapidly  and  abundantly  sol.  in  sat.  KC1+ 
Aq  with  pptn.  of  K2SO4. 
Na2SO4+10H2O  is  sol.  in  sat.  NaCl+Aq 

5.91 
6.30 
6.64 
6.90 
7.36 

0.409 
0.332 
0.297 
0.173 
0.071 

NaHS04 

NaHSO4+NaH3(SO4)2,  H2O 
NaH3(S04)2,  H20 

without  pptn.    If  effloresced  Na2SO4  is  used, 
a  ppt.  of  NaCl  is  caused  at  first,  and  subse- 
quently of  Na2SO4+10H2O.    (Karsten.) 
Sol.  in  boiling  sat.  NaCl+Aq  with  pptn.  of 
NaCl,  but  from  cold  solutions  the  Na2SO4 

7.74 

0.047 

•I 

separates  out  first.    (Vauquelin.) 

7.82 

0^044 

«. 

Less  sol.  in  NaCl  +Aq  than  in  H2O.    (Hunt, 

8.12 

0.037 

» 

Am.  J.  Sci.  (2)  25.  368.) 

8.29 
8.40 

0.042 
0.046 

,, 

Solubility  in  NaCl+Aq  at  t°. 

8.70 

0]076 

» 

g.  NaCl  per 

g.  Na2SO4  per 

8.86 

0.156 

" 

t° 

100  g.  H2Oj 

100  g.  H2O 

8.93 
8.93 

0.259 
0.269 

M 

10 

0.00 

4OQ 

9.14 

6Af) 

8.93 

0.273 

.40 

9  AH 

.<±A 
47ft 

8.84 
8.73 
8.70 

0.527 
0.681 
0.808 

NaH3(SO4)2)  H2O 

.ou 
15.65 
21.82 

.  /O 

3.99 
3.97 

4-1  f 

8.62 

0.834 

metastable  solutions 

. 

28.  13 

Of)     1  I 

.  15 
404 

8.62 

8/31 

0.844 

OOQQ 

oU.  11 

32.27 

.  Ort 

4.59 

.01 

8.87 

.o»y 
0.445 

NaH3(SO4)2,  H2O+Na2SO4, 

33.76 

4.75 

8.93 

0.437 

4.5H2SO4 
Na2S04,  4.5H2S04 

21.5 

0.00 
9.05 

21.33 
15.48 

9.08 
9.36 
9.18 

0.394 
0.425 
0.567 

Na2S04,  4.5H2S04+NaHS2O7 
NaHS2O? 

17.48 
20.41 
26.01 

13.73 
13.62 
15.05 

9.42 

0.728 

26.53 

14.44 

9.48 

0.760 

27.74 

13.39 

9.55 
9.48 
9.85 

0.775 
0.953 

0.787 

NaHS207+? 

31.25 
31.80 

QO    in 

10.64 
10.28 

Q    4Q 

9.98 

(9.77) 

0.908 
(1.03) 

Metastable 

• 

»  >_  .  xv/ 

33.69 
34.08 

O  .  "O 

4.73 

2.77 

10.16 

0.797 

35*46 

0.00 

10.78 

0.302 

? 

25 

C.OO 

28.74 

(D'Ans,  Z.  anorg.  1913,  80.  236.) 

2.74 

26.57 

8.15 

23.15 

19.86 

20.52 

24.58 

14.86 

SI.  sol.  in  cone.  HC2H3O2.     (Ure's  Diet.) 

31  21 

9.95 

Not  pptd.  by  addition  of  glacial  HC2H3O2  to 

Na2SO4+Aq.    (Persoz.) 

32]  02 

9^61 

1022 


SULPHATE,  SODIUM 


Solubility  in  NaCl+Aq  at  t°—  Continued. 

Solubility  in  NaCl+Aq  at  15°. 

t° 

g.  NaCl  per 
100  g.H2O 

g.  Na2SO4  per 
100  g.  H20 

Composition  of  the 
sat.  solution 

Solid  Phase 

27 

0.00 

2.66 
5.29 
7.90 
16.13 
18.91 
19.64 
20.77 
32.33 

31.10 
28.73 
27.17 
26.02 
24.83 
21.39 
20.11 
19.29 
9.53 

%  by  wt. 
Na2S04 

%  by  wt. 
NaCl 

11.5 
7.86 
5.87 
5.23 
5.26 
5.64 
2.26 
0 

0 
5.42 
11.51 
15.97 
21.03 
23.39 
25.21 
26.3 

Na2SO4+10H2O 

u 

It 
u 
f( 

Na2SO4,  10H2O  +  NaCl 

NaCl 

a 

30 

0.00 
2.45 
5.61 
7.91 
10.61 
12.36 
15.65 
18.44 
20.66 
32.43 

39.70 
38.25 
36.50 
35.96 
31.64 
29.87 
25.02 
21.30 
19.06 
9.06 

(Schreinemakers  and  de  Baat.  Z.  phys.  Ch. 
1909,  67.  554.) 

Sol.  in  sat.  NH4NO3+Aq.     (Margueritte, 
C.  R.  38.  307.) 
Sol.  in  sat.  KNO3+Aq  with  pptn.  after 
several  hours.    (Karsten.) 
Na2SO4+10H2O  is  sol.  in  sat.  NaNO3+Aq 
without  pptn.,  but  if  effloresced  Na2SO4  is 
used,  NaNO3  is  pptd.  at  first,  and  subse- 
quently Na2SO4+7H2O. 
The  presence  of  CaSO4  does  not  affect  the 
solubility  of  Na2SO4  in  H2O  to  any  great 
extent.       (B.arre,     A.     ch.     1911,     (8)     24. 
160.) 
More  sol.  in  K2SO4,  CuSO4,  MgSO4+Aq. 
than  in  H2O.      (Pfaff.  A.  99.  226.) 
100  pts.  H2O  dissolve  20.7  pts.  CuSO4  and 
15.9  pts.  Na2SO4.    (Rudorff,  B.  6.  484.) 
Sol.  in  sat.   MgSO4,  K2SO4,  CuSO4+Aq, 
but  if  more  Na2SO4  than  can  be  dissolved  is 
added  to  the  CuSO4+Aq,  a  large  quantity  of 
a  double  sulphate  separates  out.     (Karsten.) 
The  solubility  of  Na2SO4  in  K2SO4+Aq  has 
been  determined  at  15°,  25°,  40°,  50°,  60°,,  70° 
and  80°.    From  the  results  the  conclusion  is 
drawn  that  sodium  and  potassium  sulphates 
form  a  double  salt  of  the  formula  K3Na(SO4)2. 
(Okada,  Chem.  Soc.  1915,  108.  (2)  344.) 
See  also  under  CuSO4,  MgSO4,  and  K2SO4. 
Slowly  but  abundantly  sol.  in  sat.  ZnSO4+ 
Aq,  with  separation  of  a  double  salt  after  a 
few  days. 

33 

0.00 
1.22 
1.99 
2.64 
3.47 
12.14 
21.87 
32.84 
33.99 
34.77 

48.48 
46.49 
45.16 
44.09 
42.61 
.       29.32 
16.83 
8.76 
4.63 
2.75 

35 

0.00 
2.14 
13.57 
18.78 
31.91 
35.63 

47.94 
43.75 
26.26 
19.74 

8.28 
0.00 

At  33°  and  above  the  values  represent  the 
solubility  of  Na2SO4  in  NaCl+Aq.     At  10° 
the  solid  phase  in  contact  with  the  solution  is 
probably  Na2SO4,  7H2O.     Between  17°  and 
33°  the  solid  phase  is  either  Na2SO4,  10H2O  or 
Na2SO4.    An  inversion  of  Na2SO4,  10H2O  to 
Na2SO4  takes  place  at  various  temp,  below 
33°.  depending  on  the  amount  of  NaCl  con- 
tained in  the  solution  in  contact  with  the 
solid  sodium  sulphate. 

(Seidell,  Am.  Ch.  J.  1902,  27.  55.) 


Solubility  of  ZnSO4.7H2O+Na2SO4.10H2O  in 
100  g.  H2O  at  t°. 


t° 

grams  ZnSO4 

grams  Na2SOi 

0 
5 

40.305 
42.285 

7.905 
9.515 

(Koppel,  Z.  phys.  Ch.  1905,  62.  409.) 
See  also  under  Na2Zn(SO4)4+4H2O. 


SULPHATE,  SODIUM 


1023 


Solubility 

of    Na2SO4+Th(SO4)2     at     16°. 
Solid  phase  Th(SO4)2. 

Solubility  of  Na2SO4  in  alcohol  +Aq  at  t°, 

t° 
15 

25 

alcohol 

g.  per  100  g.  solution 

solid  phase 

Pts.  per  100  pts.  H2O 

Pts.  per  100  pts.  H2O 

H2O 

alcohol 

Na2SO4 

Na2S04 

1.094 
1.960 
2.84 
2.98 
4.11 

Th(S04)2 

Na2S04 

Th(S04)2 

0.7 
9.2 
19.4 
39.7 
58.9 
72.0 
0.0 
11.2 
20.6 
30.2 

88.7 
85.1 
78.6 
60.0 
41.1 
28.0 
72.8 
76.5 
74.3 
68.4 

0.0 
8.6 
18.9 
39.5 
58.8 
72.0 
0.0 
9.5 
19.2 
29.6 

11.3 
6.3 
2.9 
0.5 
0.1 
0.0 
27.2 
14.0 
6.5 
2.0 

Na2SO4+10H2O 

(( 
(1 

u 

Na2SO4+7H2O 
PI 

it 

1 
2 
3 
3 
3 

.743 
.387 
.800 
.962 
.375 

5.79 
9.35 
12.24 
15.36 

2.136 
1.379 
1.169 
1.048 

(Barre,  C.  R.  1911,  160.  155.) 

Solubility  in  Na  acetate  +Aq  at  25°. 
Solid  phase,  Na2SO4+10H2O. 

0.0 
10.6 
24.0 
54.0 

78.1 

78.5 
72.8 
45.6 

0.0 
9.3 
22.9 
54.0 

21.9 
12.2 
4.3 
0.4 

Na2SO4  +  10H2O 
it 

C( 

1C 

Composition  of  the  solutions 

36 
45 

0.0 

8.8 
12.8 
17.9 
18.1 
28.9 
48.7 

67.0 
70.0 
71.2 
71.1 
71.0 
66.5 
50.9 

0.0 

6.8 
10.5 
15.5 
15.7 

28.4 
48.3 

33.0 
22.6 
18.3 
13.4 
13.3 
5.1 
0.8 

Na2SO4 
tt 

it 

^< 
(( 

(L 
(I 

%  Na  acetate 

%  Na2S04 

%  H20  J0 

0 
4.10 
7.71 
12.58 
16.26 
20.63 

21 
17 
16 
13 
11 
8 

9 

72 
48 
50 
50 
10 

78.10 
78.18 
75.81 
73.92 
72.24 
71.27 

0.0 
9.0 
14.5 
20.6 
31.0 

67.6 
71.3 
71.8 
70.6 
65.6 

0.0 
7.1 
12.1 
18.4 
29.5 

32.4 
21.6 
16.1 
10.0 
4.9 

it 

It 
ie 
<t 

(C 

(Fox 

,  Chem.  Soc.  1909, 

95. 

888.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Alcohol  precipitates  Na2SO4  +  10H2O  from  the  cold 
saturated  aqueous  solution.  (Brandes  and  Firnhaber.) 

Insol.  in  alcohol  of  from  0.817  to  0.90  sp.  gr.  (Kir- 
wan.) 

1000  pts.  alcohol  of  0.872  sp.  gr.  dissolve  0.7  pt. 
Na2SO4  at  12.5-15°;  of  0.905  sp.  gr.  dissolve  3.8  pts. 
Na2S04  at  12.5-15°. 

Insol.  in  alcohol  of  0.83-0.85  sp.  gr.     (Anthon.) 

From  supersaturated  solution  in  alcohol, 
crystals  with  7H2O  are  formed.  (Schiff,  A. 
106. 11.) 

100  pts.  10%  alcohol  at  15°  contain  14.35 
pts.  Na2SO4  +  10H2O;  20%  alcohol  at  15° 
contain  5.6  pts.  Na2SO4  +  10H2O;  40%  alcohol 
at  15°  contain  1.3%  Na2SO4  +  10H2O.  (Schiff, 
A.  118.  365.) 

Very  si.  sol.  in  abs.  alcohol  at  ord.  temp.; 
somewhat  more,  though  still  exceedingly 
sparingly,  sol.  in  abs.  alcohol  acidulated  with 
H2SO4.  (Fresenius.) 

Alcohol  does  not  affect  crystal  H2O  of 
Na2SO4+10H2O. 


Between  certain  concentrations  of  alcohol, 
the  liquid  separates  into  two  layers  at  25°, 
36°  and  45°,  of  the  following  composition. 


Upper  Layer 

Lower  Layer 

t° 

nfo 

alcohol 

Na&0< 

H!O 

acohol 

Nafs04 

25 

66.5 

27.3 

6.2 

67.4 

5.1 

27.5 

68.1 

23.9 

8.0 

68.5 

6.0 

25.5 

68.3 

23.1 

8.6 

68.3 

6.7 

25.0 

36 

66.6 

4.1 

29.3 

57.7 

38.4 

3.9 

65.0 

28.3 

6.7 

68.8 

5.9 

25.3 

68.1 

21.2 

10.7 

68.9 

9.4 

21.7 

45 

61.8 

32.9 

5.3 

65.8 

25.3 

8.9 

68.4 

8.8 

22.8 

66.0 

24.0 

10.0 

68.6 

10.1 

21.3 

(de  Bruyn,  Z.  phys.  Ch.  1900,  32.  101.) 


1024 


SULPHATE,  SODIUM  HYDROGEN 


Solubility  in  alcohol  +Aq  at  25°. 

odium  thorium  sulphate,  Na2SO4,  Th(SO4)2 
+6H2O. 
Sol.  in  H2O.    100  pts.  cold  sat.  Na2SO4+Aq 
issolve  4  pts.  of  this  salt.    (Cleve.) 
See  also  under  Na2SO4+ThSO4. 

Sodium  titanium  sesgwisulphate,  Na2Ti2(SO4)4 
+5H2O. 
Sol.  in  H2O.     (Spence,  Chem.  Soc.   1904, 
86.  (2)  412.) 
Insol.  in  alcohol.     (Knecht,  B.  1903,  36. 
69.) 

Composition  of  the 
sat.  solution 

Solid  phase 

%by 
wt, 
H2O 

63.41 
49.0 
46.6 
34.9 

%by 
wt. 
alcohol 

34.84 
50.5 
53.0 
64.95 

%  by 

wt. 

Na2S04 

1.75 
0.5 
0.4 
0.15 

Na2SO4,  10H2O 

(C 

Na2SO4,  10H2O+Na2SO4 
Na2SO4 

(Schreinemakers,  Z.  phys.  Ch.  1909,  67.  552.) 

Solubility  data  for  solution  of  NaCl  in  ethyl 
alcohol +Aq.  at  15°,  25°,  and  30°  are  given  by 
Schreinemakers  (Z.  phys.  Ch.  1909,  67.  556). 

Solubility  in  propyl  alcohol +Aq  at  20°. 


%  propyl 
alcohol 

g.  Na2S04 
per  100 
g.  solution 

%  propyl 
alcohol 

g.  Na2S04 
per  100 
g.  solution 

42.20 
49.77 
55.65 

1.99 
1.15 
0.72 

56.57 
60.64 
62.81 

0.55 
0.44 
0.38 

(Linebarger,    Am.    Ch.    J.    1892,    14.    380.) 

Sol.  in  glycerine. 

Insol.  in  acetone.  (Naumann,  B.  1904  37. 
4329;  Eidmann,  C.  C.  1899.  II,  1014.); 
benzonitrile.  (Naumann,  B.  1914,  47.  1370) 
methyl  acetate.  (Naumann,  B.  1909,  42. 
7790);  ethyl  acetate.  (Naumann,  B.  1910,  43. 
314.) 

100  g.  H2O  dissolve  183.7  g.  sugar +30.5 
g.  Na2SO4  at  31.25°,  or  100  g.  sat.  solution 
contain  52.2  g.  sugar  +  9.6  g.  Na2SO4 
(Kohler,  Z.  Ver.  Zuckerind,  1897,  47.  447. 

Min.  Anhydrous,  Thenardite.  +  10H2O 
Mirabilite. 

Sodium  hydrogen  sulphate,  NaHS04. 

Not  deliquescent.  Very  sol.  in  H2O  with 
decomposition. 

Sol.  in  2  pts.  H2O  at  0°  (Link);  1  pt.  H2C 
at  100°  (Schubarth).  100  pts.  H2O  at  15.5C 
dissolve  92.72  pts.  Sol.  in  2  pts.  H2O  at 
18.75°  (Abl)j  decomp.  by  alcohol. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch 
J.  1898,  20.  829  ) 

+H2O.  Deliquescent,  and  decomp.  by  the 
H2O  which  it  takes  up. 

NaH3(SO4)2.    Decomp.  by  H2O.    (Schultz. 

Tnsodium  hydrogen  sulphate,  NasH(S04)2. 
Sol.  in  H2O  with  decomp. 
+H2O.    (Rose.) 

Sodium  pi/rosulphate,  Na2S2O7. 

Sol.  in  fuming  H2SO4  without  decomp. 

Sodium  thallic  sulphate,  Na2SO4,  T12(SO4),. 
Sol.  in  H2O.    (Strecker,  A.  136.  207.) 


Sodium   titanyl   sulphate,    Na2TiO2(S04)2+ 

10H2O. 

Hygroscopic.    (Mazzuchelli  and  Pantanelh, 
.  C.  1909,  II.  420.) 

Sodium  uranyl  sulphate,  Na2(UO2)(S04)2+ 

3H20. 
(de  Coninck,  C.  C.  1906,  I.  919.) 


Sodium  vanadium  sulphate,  Na2V2(S04)4+ 

24H2O. 

Very  sol.  in  H2O.    (Piccini,  Z.  anorg.  1897, 
13.  444.) 


Sodium  vanadyl  sulphate,  Na2S04,  VOSO4+ 
4H20. 

Easily  sol.  in  H2O  and  alcohol  +  cone. 
H2SO4.  (Koppel,  Z.  anorg.  1903,  36.  177.) 

Na2SO4,  2VOSO4+2^H2O.  Slowly  sol. 
inH2O. 

Can  be  cryst.  from  H2SO4  at  100°.  (Kop- 
pel.) 

Sodium  yttrium  sulphate,  Na2S04,  Y2(S04)8+ 
2H2O. 

Quite  sol.  in  H2O.    (Cleve.) 

The  only  double  salt  capable  of  existing 
at  25°.  (James  and  Holden,  J.  Am.  Chem. 
Soc.  1913,  36.  562.) 

Sodium  zinc  sulphate,  Na2SO4,  ZnS04+ 
4H2O. 

Deliquescent  in  moist  air. 

Decomp.  into  constituents  on  dissolving  in 
H2O.  (Graham,  Phil.  Mag.  18.  417.) 

Solubility  of  Na2Zn(SO4)2.+4H2O   in  100  g. 
H2O  at  t°. 


t 

grams  ZnSO4 

grams  Na2SO4 

25 
30 
35 
40 

26.32 
26.475 
26.365 
26.68 

23.40 
23.445 
23.525 
23.63 

(Koppel,  Z.  phys.  Ch.  1905,  62.  409.) 

SULPHATE,  STRONTIUM 


1025 


Solubility  of  Na2Zn(SO4)2.4H2O+ZnSO4. 
7H2O  in  100  g.  H2O  at  t°. 

Sol.  in  about  8000  pts.  H2O.     (Schweitzer, 
J.  B.  1877.  1054.) 
Calculated  from  electrical  conductivity  of 
the  solution,  SrSO4  is  sol.  in  10,070  pts.  H2O 
at  16.1°  and  10,090  pts.  at  20.1*.    (Holleman, 
Z.  phys.  Ch.  12.  131.) 
1  1.  H2O  dissolves  107  mg.  SrSO4  at  18°  and 
not  much  more  at  higher  temp.    (Kohlrausch 
and  Rose.  Z.  phys.  Ch.  12.  241.) 
100  g.  H2O  dissolve 
att°            0°-5°      10°-12°      20°           30° 
g.  SrSO4     0.0983     0.0994     0.1479      1.0600 

t° 

grams 
ZnSCU 

grams 
Na2S04 

t° 

grams 
ZnSO4 

grams 
Na2S04 

10 
15 

20 

45.79 
48.81 
52.34 

11.24 
10.175 
8.625 

25 
30 
35 

56.155 
60.55 
65.25 

7.215 
6.34 
5.64 

(Koppel.) 

Solnhilitv    of    TV"n^7nCSn^»  4TT«n-l_7T,SO. 

on2u  in  iwu  g.  n.2\j  at  t  . 

att°              50°          80°          90°        95-98° 
g.  SrSO4     0.1629     0.1688     0.1727      0.1789 
(Wolfrnann,  C.  C.  1897,  1.  632.) 

1  1.  H2O  dissolves  114  mg.  SrSO4  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1904,  60.  356.); 
114.3  mg  at  18°.     (Kohlrausch,  Z.  phys.  Ch. 
1908,  64.  168.) 
Sol.  in  6895  pts.  cold,  and  9638  pts.  boiling 
H2O;  in  11,000-12,000  pts.  H2O  containing 
H2SO4;   in   474   HCl+Aq   containing  8.5% 
HC1;  in  432  pts.  HNO3+Aq  containing  4.8 
%  N2O6;  in  7843  pts.  HC2H3O2+Aq  contain- 
ing 15.6%  HC2H3O2.    (Fresenius.) 
Or,  1  1.  cold  HCl+Aq  of  8.5%  dissolves  2.11 
g.  SrSO4;  1  1.  cold  HNO3+Aq  of  4.8%  N2O5 
dissolves  2.31  g.  SrS04;  1  1.  cold  HC2H3O2  + 
Aq  of  15.6%  HC2H3O2  dissolves  0.1275  g. 
SrSO4.    (Fresenius.) 

Solubility  of  SrSO4  in  HCl+Aq. 

t 

grams  ZnSCh 

grams  NazSCh 

38 
40 

66.64 
64.89 

4.98 
4.71 

(Koppel.) 

Solubility     of     Na2Zn(SO4)2.4H2O+Na2SO4. 
10H2O  in  100  g.  H2O  at  t°. 

t° 

grams  ZnSCU 

grams  NassSCh 

10 
15 
20 
25 
30 

43.495 
36.925 

28.77 
19.935 
10.67 

12.35 
16.71    ' 
21.98 
29.875 
42.515 

(Koppel.) 

Solubility     of     Na2Zn(SO4)2.4H2O+Na2SO4 
(anhydrous)  in  100  g.  H2O  at  t°. 

No.  cc.  HC1  + 
Aq  containing 
1  mg.  equiv.  HC1 

g.  per  100  cc.  solution 

t° 

grams  ZnSCh 

grams  Na2SO4 

HC1 

SrS04 

35 
40 

8.725 
9.16 

46.61 
43.835 

0.2 
0.5 
1.0 
2.0 
10.0 

18.23 
7.29 
3.65 
1.82 
0.36 

0.161 
0.207 
0.188 
0.126 
0.048 

(Koppel.) 

Sodium  sulphate  fluoride,  Na2SO4,  NaF. 
Cryst.  from  H2O  without  decomp.     (Marig- 
nac,  Ann.  Min.  (5)  16.  236.) 

Sodium  sulphate  antimony  /'/•/fluoride. 
See  Antimony  /nfluoride  sodium  sulphate. 

Strontium  sulphate,  SrSO4. 
Very  si.  sol.  in  cold,  and  still  less  in  boiling 
H2O. 
1  1.  H2O  at  11-15°  dissolves  0.066  g.  SrSO4 
(Brandes  and  Silber);  0.145  g.  SrSO4  (Fre- 
senius);   0.154-0.167   g.    SrSO4    (Marignac); 
0.187  g.   SrSO4   (Kremers);  0.278  g.   SrSO4 
(Andrews)  . 
1  1.  boiling  H2O  dissolves  0.104  g.  SrSO4 
(Fresenius);   0.282   g.    SrSO4    (Brandes   and 
Silber). 
When  a  Sr  salt  is  precipitated  by  H2SO4,  1 
pt.  SrSO4  remains  dissolved  in  700  pts.  H2O. 
(Marignac.) 

(Banthisch,  J.  pr.  1884,  (2)  29.  54.) 
Solubility  of  SrSO4  in  HNO3+Aq. 

No.  cc.  HN08  + 
Aq  containing 
1  mg.  equiv. 
MN03 

g.  per  100  cc.  solution 

HNOa 

SrSO4 

0.2 
0.5 
1.0 
2.0 
10.0 

31.52 
12.61 
6.30 
3.15 
0.63 

0.381 
0.307 
0.217 
0.138 
0.049 

(Banthisch,  J.  pr.  1884,  (2)  29.  54.) 

Sol.  in  cone.  H2SO4.    See  under  SrH2(SO4)2. 
Insol.  in  NH4Cl+Aq  or  cone.  (NH4)2SO4+ 
Aq.    (Rose.) 
Slowly  but  completely  sol.  in  NaCl+Aq. 
(Wackenroder.) 
H2O  containing  Na2SO4  dissolves  less  SrSO* 

1026 


SULPHATE,  STRONTIUM  HYDROGEN 


than  pure  H2O;  H2O  containing  H2SO4  still 
less.  (Andrews,  Phil.  Mag.  Ann.  7.  406.) 

Insol.  in  Na2S2O3+Aq. 

Insol.  in  boiling  cone.  (NH4)2SO4-|-Aq. 
(Rose,  Pogg.  110.  292.) 

Sol.  in  16.949  pts.  (NH4)2SO4+Aq  (1:4). 
(Fresenius,  Z.  anal.  32.  195.) 

Pptn.  is  hindered  by  alkali  metaphosphates 
and  citrates,  but  not  by  citric  acid. 

Decomp.  at  ord.  temp.,  and  more  rapidly 
on  boiling  by  alkali  carbonates +Aq. 

Sol.  in  MgCl2  or  KCl+Aq,  solubility  in- 
creasing with  strength  of  solution;  sol.  in 
NaCl  or  CaCl2+Aq  maximum  solubility 
occurring  when  the  solutions  are  of  a  medium 
concentration.  The  numerical  results  are  as 
follows: 

100  pts.  of  the  salt  solutions  containing  given 
pts.  salt  dissolve  pts.  SrSO4. 


Salt 

Pts.  salt 

Pts.  SrS04 

NaCl 

22.17 
15.54 
8.44 

0.1811 
0.2186 
0.1653 

KC1 

18.08 
12.54 

8.22 

0.2513 
0.1933 
0.1925 

MgCl2 

13.63 
4.03 
1.59 

0.2419 
0.2057 
0.1986 

CaCl2 

33.70 
16.51 

8.67 

0.1706 
0.1853 
0.1756 

(Virck,  C.  C.  1862.  402.) 


Solubility  in  H2O,  and  in  solutions  of  the 
sulphates  chlorides  and  nitrates  of  the 
alkalies  and  alkaline  earths  and  in  solutions  of 
salts  of  the  alkalies  with  strong  organic  acids 
has  been  determined.  No  data  in  abstract 
(Wolfmann,  Chem/  Soc.  1898,  (2)  74.  220.) 

Solubility  in  H2O  is  considerably  decreased 
by  the  presence  of  K2SO4.  (Barre,  A.  ch. 
1911,  (8)  24.  175.) 


Solubility  of  SrSO4  in  Ca(NO3)2+Aq  at  ord. 

temp. 
G.  per  100  cc.  sat.  solution. 


Ca(NOa)2 

SrS04 

Ca(N03)2 

SrS04 

0.5 
1 
2 
3 

0.0483 
0.0619 
0.1081 
0.1275 

4 
5 
6 

0.1489 
0.1689 
0.1955 

(Raffo  and  Rossi,  Gazz.  ch.  it.  1915,  46.  (1) 
45.) 


Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

100  g.  95%  formic  acid  dissolve  0.02  g. 
SrSO4  at  18.5°.  (Aschan,  Chem.  Ztg.  1913. 
37.  1117.) 

Insol.  in  absolute  alcohol;  scarcely  sol.  in 
dil.  alcohol. 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  acetone.  (Naumann,  B. 
1904,  37.  4329;  Eidmann,  C.  C.  1899,  II. 
1014.) 

Min.  Celeslite. 

Strontium  hydrogen  sulphate,  SrH2(SO4)2. 

100  pts.  H2SO4  dissolve  2.2  pts.  SrSO4  (Lies- 
Bodart  and  Jacquemin);  100  pts.  H2SO4  dis- 
solve 5.68  pts.  (Struve,  Z.  anal.  9.  34);  100 
pts.  fuming  H2SO4  dissolve  9.77  pts. 
(Struve). 

1  g.  SrSO4  dissolves  in  1256  g.  91%  H2SO4+ 
Aq  (Varenne  and  Pauleau,  C.  R.  93.  1016); 
boiling  H2SO4  dissolves  about  15%  SrSO4,  and 
still  more  at  100°.  (Schultz,  Pogg.  133.  147). 

Sol.  in  1519  pts.  91%  H2SO4.  (Varenne 
and  Pauleau,  C.  R.  93.  1016.) 

100  pts.  H2SO4  (sp.  gr.  1.843)  dissolve  14 
pts.  SrSO4  at  70°.  (Garside,  C.  N.  31.  245.) 

Decomp.  by  H2O. 

100  pts.  hot  cone.  H2SO4  dissolve  about 
9.0  pts.  SrSO4.  (Rohland,  Z.  anorg.  1910, 
66.  206.) 

10  ccm.  of  sat.  SrSO4+absolute  H2SO4 
contain  approx.  2.17  g.  SrSO4.  (Bergius,  Z. 
phys.  Ch.  1910,  72.  355.) 

+H2O.    Decomp.  by  H2O. 

Strontium    tin    (stannic)    sulphate,    SrSO4. 

Sn(SO4)2+3H2O. 

Decomp.  by  H2O.  Sol.  in  HC1.  (Wein- 
land  and  Kiihl,  Z.  anorg.  1907,  54.  249.) 

Strontium  titanium  sulphate,  SrSO4,  Ti(SO4)2. 

Ppt;  decomp.  by  H2O  giving  titanic  acid. 

(Weinland  and  Kiihl,  Z.  anorg.  1907,  64.  254.) 

Tantalum  sulphate,  3Ta2O6,  SO3+9H2O. 
(Hermann,  J.  pr.  70.  201.) 

Tellurium  sulphate,  basic,  TeO2,  SO3. 

Sol.  in  cold  dil.  H2SO4.  Decomp.  by  hot 
H2O.  (Klein,  C.  R.  99.  326.) 

Terbium  sulphate,  Tr2(SO4)3+8H2O. 

Sol.  in  H2O. 

Sol.  in  H2O;  pptd.  by  alcohol.  (Urbain,  C. 
R.  1908,  146.  127.) 

Thallous  sulphate,  T12SO4. 

1  pt.  dissolves  at  t°  in  pts.  H2O,  according 
to  C  =  Crookes;  L  =  Lamy : 

15°      18°     62°     100°     101  2° 

21.1     20.8    8.7      5.4       5.22  pts.  H2O. 


SULPHATE,  THORIUM 


1027 


Solubility  of  T12SO4  in  H2O. 

T12SO4,  T1HSO4.     Sol.  in  H2O. 
KooL-or-  "p   f  /»  1  ono  01   on  ^ 

(Storten- 

t° 

%  T1.S04 

t° 

%  T12SO, 

oecKer,  it.  t.  c.  lyuz,  &L.  yu.j 

0 
10 

2.63 
3.57 

60 
70 

9.85 
11.31 

Thallous  p?/r0sulphate,  Tl2S2O7. 
Decomp.  by  H2O.     (Weber,  B. 

17.  2502.) 

20 
30 

4.64 
5.80 

80 
90 

12.75 
14.19 

Thallous  ortosulphate,  TkS8O25. 

40 

7.06 

99.7* 

15.57 

Decomp.  by  H2O.     (Weber,  B. 

17.  2502.) 

50 

8.44 

. 

Thallic  sulohate.  basic.  Tl,O,.  2SC 

,4-3H,O. 

B.-pt.  at  748  mm. 

(Berkeley,  Phil.  Trans.  Roy.  Soc.  1904,  203. 
A,  189;  calc.  by  Landolt-Bornstein.) 

100  g.  H2O  dissolve  3.36  g.  T12SO4  at  6.5°; 
4.3  g.  at  12°;  19.14  g.  at  100°.  (Tutton,  Proc. 
Roy.  Soc.  1907,  79.  A,  351.) 

1  1.  H2O  dissolves  0.1928  equivalents 
T12SO4  at  20°,  or  48.59  g.  in  1  1.  of  solution. 
(Noyes,  J.  Am.  Chem.  Soc.  1911,  33.  1657.) 

1  1.  H20  dissolves  0.1083  g.  equiv.  T12SO4 
at  25°,  or  27.28  g.  in  1 1.  of  solution.  (Noyes.) 

Solubility  in  H2SO4+Aq  at  25°. 


Strength  of  H  SOi  +Aq 
g.  mols.  per  1. 

g.  mols.  Tl  SO4  per  1. 

0.0494 
0.0987 

0.1172 
0.1249 

(Noyes,  J.  Am.  Chem.  Soc.  1911,  33.  1662.) 

1  1.  TIClOs+Aq.  containing  0.1058  equiv- 
alents T1C1O3,  dissolves  0.1366  equivalents 
Tl2SO4at20°.  (Noyes.) 

See  also  T1C1O3. 

Solubility  in  salts +Aq  at  25°. 


g.  mols.  per  1. 

'g.  mols.  per  1.  Tl  SO4 
dissolved 

0.0996T1NO3 
0.0497Na2SO4 
0.1988Na2SO4 
0.1010NaHSO4 

0.08365 
0.1080 
0.1173 
0.1161 

(Noyes.) 

Thallous  hydrogen  sulphate,  T1HSO4. 

SI.  hydroscopic. 

Solubility  in  H2SO4+Aq  at  25°. 

1000  g.  of  the  solution  contain: 


Mols.  HzSCh 

Mols.  T12SO4 

4.55 

0.56 

4.79 

0.55 

4.89 

0.59 

4.92 

0.66 

4.78 

0.75 

4.26 

1.01 

4.03 

1.08 

(D'Ans,  Z.  anorg.  1910,  66.  232.) 


Sol.  in  H2O. 

+5H2O.    As  above.     (Willm,  A.  ch.  (4)  5. 

5.) 

Thallic  sulphate,  T12(SO4)3+7H2O. 

Decomp.  by  cold  H2O  with  separation  of 
TIO(OH).  (Crookes.) 

Thallothallic  sulphate,  2T12O,  3T12O3,  12SO3+ 

25H20. 

Gradually  efflorescent.    (Willm.) 
-T12(SO4)2.      (Lepsius,    Chero.    Ztg.    1890. 

1327.) 
T1H(SO4)2.    (Lepsius.) 

Thallous  uranyl  sulphate,  Tl2(UO2)(SO4)2-f- 
3H20. 

SI.  sol.  in  cold  H2O. 

Easily  forms  supersat^  solutions..  (Kohn, 
Z.  anorg.  1908,  59.  112.) 

Thallium  vanadium  sulphate,  T12V2(SO4)4  + 
24H2O. 

100  pts.  H2O  dissolve  11.06  pts.  salt  at  10°. 

Sp.  gr.  of  solution  at  4°/20°  =  2,342. 

Very  sol.  in  hot  H2O.  (Piccini,  Z.  anorg. 
1897,  13.  446.) 

256  g.  anhydrous,  or  433  g.  hydrated  salt, 
or  0.573  g.  mols.  of  anhvdrous  salt  are  sol.  in 
1  1.  H2O  at  25°. 

Melts  in  crystal  H2O  at  48°.  (Locke,  Am. 
Ch.  J.  1901,  26.  175.) 

Thallous  zinc  sulphate,  Tl2Zn(SO4)2+6H2O. 

1  1.  H2O  dissolves  86  g.  anhydrous  salt 
at  25°.  (Locke,  Am.  Ch.  J.  1902,  27.  459.) 

Thallothallic  sulphate  bromide,  Tl2Br2SO4. 

Very  sol.  in  cold  H2O.  Decomp.  by  much 
H2O.  (Meyer  and  Goldschmidt,  B.  1903,  36. 

242.) 

Thorium  sulphate,  basic,  3[Th(SO4)2+2H2O], 
Th(SO4)0+2H2O. 

Insol.  in  H2O;  very  slowly  attacked  by  dil. 
acids.  (Demarcay.) 

ThO(SO4)+2H2O.  Stable  in  aq.  solution 
at  100°.  (Hauser,  B.  1910,  43.  2776.) 

+5H2O.  Somewhat  sol.  in  hot  cone. 
MgSO4+Aq.  (Halla,  Z.  anorg.  1912,  79.  260.) 

Thorium  sulphate,  Th(SO4)2. 

Anhydrous.  Easily  sol.  if  brought  into  a 
large  amount  of  H2Q,  but  very  slowly 'sol.  if 
only  a  little  H20  is  added  to  the  salt. 


1028 


SULPHATE,  THORIUM 


100  pts.  H2O  dissolve  about  4.86  pts. 
Th(SO4)2  at  0°.  (Cleve.) 

When  heated,  a  hydrous  salt  separates  out, 
which  redissolves  on  cooling.  (Cleve.) 

Solubility  of  anhydrous  salt  cannot  be 
determined,  as  it  begins  to  separate  out 
Th(SO4)2+9H2O  before  a  saturated  solution 
is  reached.  At  0°,  100  pts.  H2O  dissolved  22.97 
pts.  Th(SO4)2  in  15  minutes;  at  25°,  27.00  pts. 
Th(SO4)2  were  dissolved  in  5  minutes. 
(Roozeboom,  Z.  phys.  Ch.  5.  198.) 

+2H2O.  Shows  same  behaviour  as  anhy- 
drous salt.  100  pts.  H2O  dissolved  35.50  pts. 
Th(SO4)2  from  this  salt  at  1°,  but  this  is  not 
the  maximum  solubility.  (Roozeboom.) 

+4H2O.  Pptd.  by  alcohol  from  hot  aque- 
ous solution;  also  formed  by  heating  Th(SO4)2 
-f-9H2O  in  aqueous  solution  above  60°. 

100  pts.  H2O  dissolve  pts.  Th(SO02-HH2O, 
calculated  as  Th(SO4)2,  at  t°.  D  =  ac- 
cording  to  Demarcay  (C.  R.  96.  1860); 
R=  according  to  Roozeboom  (Z.  phys. 
Ch.  6.  202). 


t° 

Pts. 

Th  (SO4)2 

t° 

Pts. 

Th  (SO4)2 

t° 

Pts. 

Th(S04)2 

17 
35 
40 

9.41  D 
4.  SOD 
4.04R 

50 
55 
60 

2.54    R 
1.94    D 
1.634  R 

70 
75 
95 

1.09R 
1.32D 
0.71  D 

+6H2O.     Behaves  as  the  anhydrous  salt, 
but  action  is  much  slower. 

100  pts.  H2O  dissolve  pts.  Th(SO4)2-|-6H2O, 
calculated  as  Th(SO4)2,  at  t°. 


Pts. 

Pts. 

Th(SO4)2 

Th  (SO4)2 

0 

1.50 

45 

3.85 

15 

1.63 

60 

6.64 

30 

2.45 

(Roozeboom.) 

This  determination  gives  too  low  figures, 
especially  at  the  higher  temperatures.  (Rooze- 
boom.) 

+8H2O. 

100  pts.  H2O  dissolve  pts.  Th(SO4)2+8H2O, 
calculated  as  Th(SO4)2.  at  t°. 


t° 

Pts. 

Th(S04)2 

t° 

Pts. 
Th(S04)» 

0 
15  . 

1.00 
1.38 

25 

44 

1.85 
3.71 

(Roozeboom.) 

100  g.  Th(SO4)2+Aq  sat.  with  Th(SO4)2+ 
8H2O  at  30°  contain  2.152  g.  anhydrous 
Th(SO4)2.  (Koppel  and  Holzkampf,  Z. 
anorg.  1910,  67.  274.) 

100  g.  H2O  dissolve  1.722  g.  at  25°.  (Barre, 
Bull.  Soc.  1912,  (4).  11.) 

+9H2O.      Pptd.    by    alcohol    from    cold 


t 

0 
10 
20 

Pts. 

Th(S04)2 

t 

Pts. 

Th(S04>2 

t° 

Pts. 
Th(S04)2 

0.88 
1.02 
1.25 

30 
40 

1.85 
2.83 

50 
55 

4.86 
6.5± 

aqueous  solution.    Sol.  in  about  88  pts.  H2O 
atO°.    (Cleve.)    Extremely  slowly  sol.  in  H20. 

100  pts.  H2O  dissolve  pts.  Th(SO4)2+9H20, 
calculated  as  Th(SO4)2,  at  t°. 


Above  55°,  Th(SO4)2+4H2O  separates  out. 

(Demarcay  C.  R.  96.  1860,  calculated  by 

Roozeboom.) 

100  pts.  H2O  dissolve  pts.  Th(SO4)2+9H20, 
calculated  as  Th(SO4)2,  at  t°. 


t° 

Pts. 
Th  (SO4)2 

t° 

Pts. 

Th(SO4)2 

t° 

Pts. 

Th(S04)2 

0 
10 
20 

0.74 
0.98 
1.38 

30 
40 

1.995 
2.998 

51 
55 

5.22 
6.76 

Above  60°,  Th(fcO4)2+4H2O  separates  out. 
(Roozeboom,  Z.  phys.  Ch.  6.  201.) 

For  further  data,  see  Roozeboom  (Z.phys. 
Ch.  6.  198),  where  there  is  a  full  discussion 
of  the  subject. 

100  g.  sat.  solution  of  Th(SO4)2+9H2O  in 
H2O  at  25°  contain  1.593  g.  anhyd.  salt. 
(Wirth,  Z.  anorg.  1912,  76.  174.) 

Solubility  of  Th(SO4)2  in  H2SO4-(-Aq  at  tc 


t° 

%  H2S04 

%  ThS04 

Solid  phase 

30 

0.000 

2.152 

Th(S04)2+8H20 

0.466 

2.055 

« 

0.72 

2.085 

« 

1.468 

2.267 

(( 

2.983 

2.311 

(C 

4.38 

2.367 

« 

4.97 

2.323 

H 

9.95 

1.961 

<( 

15.03 

1.484 

{( 

18.95 

1.078 

u 

23.64 

0.7196 

" 

32.68 

0.3364 

Th(SO4)2+4H2O 

37.80 

0.077 

n 

43.28 

0.0213 

»            u 

45.69 

0.0047 

« 

74.0 

0.1208 

C( 

80.5.    . 

0.000 

u 

20 

5 

1.722 

Th(SO4)2+8H2O 

15 

0.9752 

(C 

25 

0.3838 

K 

40 

0.0103 

Th(SO4)2+4H2O 

Boiling 

5 

0.7407 

ts 

temp. 

10 

0.4808 

(t 

15 

0.3882 

M 

(Koppel  and  Holzkampf,  Z.  anorg.  1910,  67. 
274.) 


SULPHATE,  TITANIUM  HYDROGEN 


1029 


Solubility  in  H2SO4+Aq  at  25' 


Per  100  g.  of  solution 


g.  Th(SO4)2 

g.  H2S04 

1.722 

0.000 

1.919 

1.072 

2.017 

1.941 

2.060 

2.821 

2.061 

3.843 

2.035 

5.212 

1.863 

8.055 

1.702 

10.105 

(Barre,  Bull.  Soc.  1912,  (4)  11.  647.) 
Solubility  in  H2SO4+Aq  at  25°. 


Normality 
H2S04 

In  100  g.  of  the 
liquid  are  dissolved 

Solid  phase 

g.  oxide 

anhydrous 
sulphate 

0 
1.1 

2.16 
4.32 
6.68 
9.68 
10.89 
15.15 

1.015 
1.14 
0.9265 
0.545 
0.2685 
0.0651 
0.0396 
0.0192 

1.593 
1.831 

1.488 
0.8751 
0.4312 
0.1045 
0.0636 
0.0308 

Th(S04)2+9H20 
a 

a 

<( 

Th(SO4)2+8H2O 
Th(SO4)2+4H2O 

(Wirth,  Z.  anorg.  1912,  76.  186.) 
Solubility  of  Th(SO4)2  in  HCl+Aq  at  30°. 


%HC1 


0.0 
4.55 
6.95 
12.14 
15.71 
18.33 
20 
23.9 


2.15 

3.541 

3.431= 

2.811 

2.360 

2.199 

2.13 

1.277 


Solid  phase 


Th(SO4)2+8H2O 


Th(S04)2+4H20 


(Koppel  and  Holzkampf,  Z.  anorg.  1910,  67 

274.) 

Solubility  of  Th(SO4)2  in  HNO3+Aq  at  30° 


%  HNOs 

%  Th(S04)2 

Solid  phase 

0.0 
5.17 
10.04 

16.68 
21.99 
28.33 
28.51 
33.17 
38.82 

2.15 

3.68 
4.20 
4.84 
4.47 
3.96 
3.88 
3.34 
2.51 

Th(SO4)2+8H2O 

ti 
({ 

{( 
11 

Th(SO4)2+4H2O 

(Koppel  and  Holzkampf,  Z.  anorg.  1910,  67. 

274.) 

The  presence  of  phosphoric  acid  increases 
;he  solubility  of  thorium  sulphate  in  HC1  and 
HNO3.  (Koppel  and  Holzkampf,  Z.  anorg. 
1910,  67.  280.) 

For  solubility  of  Th(SO4)2  in  (NH4)2SO4, 
i2SO4,  and  K2SO4,  see  respective  sulphates. 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  830.) 

Thorium  hydrogen  sulphate,  ThH2(SO4)3. 

Hydroscopic. 

Sol.  in  excess  of  hot  H2SO4;  insol.  in  cold 
H2SO4.  (Brauner,  Z.  anorg.  1904,  38.  333.) 

Thulium  sulphate,  Tm2(SO4)3-f  8H2O. 

Insol.  in  alcohol.  (James,  J.  Am.  Chem. 
Soc.  1911,  33.  1343.) 

Tin   (stannic)    sulphate,   basic,   (SnO)SO4+ 

H2O. 

Easily  sol.  in  cold  H2O,  but  quickly  de- 
comp. with  separation  of  stannic  hydroxide. 
(Ditte,  C.  R.  104.  178.) 

3SnO,  SO3.  Easily  sol.  in  dil.  acids. 
(Ditte,  A.  ch.  1882,  (5)  27.  159.) 

LKH2O.     Not  decomp.   by   cold  H2O. 
(Ditte.)" 

Tin  (stannous)  sulphate,  SnSO4. 

Sol.  in  5.3  pts.  H2O  at  19°,  and  5.5  pts.  at 
100°.  (Marignac.)  Solution  soon  decomposes 
with  separation  of  a  basic  salt.  Sol.  in. 
H2SO4+Aq.  (Bouquet.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.)  . 

Tin  (stannic)  sulphate,  Sn(SO4)2+2H2O. 

Deliquescent.  Easily  sol.  in  H2O;  decomp. 
by  much  H2O.  Sol.  in  dil.  H2SO4+Aq. 
Slowly  sol.  in  HCl-(-Aq.  Decomp.  by  abso- 
lute alcohol.  (Ditte,  C.  R.  104.  178.) 

Titanium  sulphate,  Ti(SO4)2+3H2O. 

Deliquescent,  and  sol.  in  H2O.  The  aque- 
ous solution  is  decomp.  on  boiling.  (Glatzel, 
B.  9.  1833.) 

Titanium  sesgm'sulphate,  Ti2(SO4)8. 

Very  deliquescent,  and  easily  sol.  in  H2O. 
Aqueous  solution  is  decomp.  by  boiling. 
(Ebelmen.) 

Insol.  in  H2O,  alcohol,  ether  and  cone. 
H2SO4.  Slowly  sol.  in  dil.  H2SO4.and  HC1. 
(Stabler,  B.  1905,  38.  2624.) 

Not  sol.  in  alcohol.  (Knecht,  B.  1903,  36. 
169.) 

+8H2O.  Sol.  in  H2O.  (Glatzel,  B.  9. 
1833.) 

Titanium  hydrogen  ses^uisulphate,  3Ti2(SO4)  j, 
H2SO4+25H2O. 

Gradually  sol.  in  H2O. 

Insol.  in  60%  H2SO4,  alcohol,  ether  and 
glacial  acetic  acid.  (Stahler,  B.  1905,  38. 
2621.) 


1030 


SULPHATE,  TITANYL 


Titanyl  sulphate,  (TiO)SO4. 

Decomp.  by  H2O.  Slowly  sol.  in  cold, 
rapidly  in  warm  HCl+Aq.  (Mer/,  J.  pr. 
99.  157.) 

+2H20.  Sol.  in  HaO.  (Blondel,  Bull. 
Soc.  1899,  (3)  21.  262.) 

2TiO2,  3SO3+3H2O.  Sol.  in  H2O  acidified 
with  HC1.  (Blondel,  Bull.  Soc.  1899,  (3)  21. 
262.) 

5Ti02,  SO3+5H2O.    (Blondel.) 

7TiO2,  2SO3+a;H2O.    (Blondel.) 

2TiO2,  SO3+zH2O.    (Blondel.) 

Uranous  sulphate,  basic,  U(OH)2SO4+H2O. 

Insol.  in  H2O.  H2O  dissolves  out  H2SO4. 
(Ebelmen,  A.  ch.  (3)  6.  217.) 

+5H2O.    Sol.  in  alcohol. 

Pptd.  by  ether.  (Rosenheim,  Z.  anorg. 
1901,  26.  251. 

Uranous  sulphate,  U(SO4)2+4H2O. 

Sol.    in    H2O    with    immediate    decomp. 

Easily  sol.  in  dil.  H2SO4+Aq.  (Kohl- 
schiitter,  B.  1901,  34.  3629.) 

Decomp.  by  H2O  into  insol.  basic,  and  sol. 
acid  salt.  Sol.  in  dil.  H2SO4  or  HCl+Aq. 
Difficultly  sol.  in  cone,  acids.  (Ebelmen,  A. 
ch.  (3)  6.  215.) 


Solubility  of  U(SO4)2+4H2O  in  H2O  at  t°. 

t°  %U(S04)2     I       t°          %U(S04)2 


29 
37 


9.8 
8.3 


8.1 
7.3 


(Giolitti  and  Bucci,  Gazz.  ch.  it.  1905,  35. 
(2)  162.) 

1  pt.  is  sol.  in  4.23  pts.  H2O  at  13°;  4.3  pts. 
at  11.3°;  4.4  pts.  at  9.1°.  (de  Coninck,  A.  ch. 
1903,  (7)  28.  12.) 

+8H2O. 

Solubility  of  U(SO4)2+8H2O  in  H2O  at  t°. 


t° 

%U(S04)2 

t° 

%  U(S04)2 

18 
25.6 
37 

10.17 
13.32 
19.98 

48.2 
62 
93 

28.72 
36.8 
63.2 

(Giolitti  and  Bucci,  Gazz.  ch.  it.  1905,  35. 
(2)  162.) 

Sp.gr.  of  U(S04)2+Aq  at  t°. 


t° 

%  salt 

Sp.  gr. 

16 

1 

1.0058 

16.8 

2 

1.0107 

16 

3 

1.0165 

17.8 

4 

.0218 

17.2 

5 

.0272 

18 

6 

.0320 

18.3 

7 

.0379 

17.4 

8 

.0429 

15.2 

9 

.0485 

15.6 

10 

.0539 

(de  Coninck,  A.  ch.  1903,  (7)  28.  11.) 


Solubility  in  acids +Aq. 
1  pt.  U(SO4)  is  sol.  in  pts.  acid  at  t°. 


9.7 
9.2 


11.2 
10.3 

11.4 
10.7 


15 
14.2 


15.5 
14.4 


16.5 
15.9 


11.7 

10.9 

10.1 

9 


Acid 


HC1 


HNO3 


H2SeO4 

(sp.  gr.  1.4) 


UBr 


HC2H3O2 


H2S04 


Concentra-          Pts. 
tion  of  acid  acid 


1:4 
1:4 

u 

1:4 


1:4 


1:4.5 


1:2 


1:4 


5.74 

5.8 


5.4 
5.53 


4.57 
4.66 


4  - 
4.23 


4.1 
4.3 


3.72 

3.85 


6.36 
6.42 
6.45 
6.5 


(de  Coninck,  Chem.  Soc.  1902,  82.  (2)  459.) 

Sp.  gr.  of  U(SO4)2+HCl(d  =  1.046)  at  t°. 
di  =  Sp.  gr.  referred  to  H2O. 
d2  =  Sp.  gr.  referred  to  HC1. 


t° 

%  salt 

d! 

d2 

16 
17 
18 
18.4 
17.6 

1 

2 
3 
4 
5 

1.0525 
1.0572 
1.0619 
1.0667 
1.0714 

1.0063 
1.0109 
1.0154 
1.0199 
1  .0243 

(de  Coninck,  A.  ch.  1903,  (7)  28.  11.) 

Sp.  gr.  of  U(SO4)2+H2SO4(d  =  1.14)  at  t 
di  =  Sp.  gr.  referred  to  H2O. 
d2  =  Sp.  gr.  referred  to  H2SO4. 


1  t° 

%salt 

d! 

d2 

18.7 
18.3 
17.4 
17.6 
18.1 

1 

2 
3 
4 
5 

1  .  1442 
.  1.1494 
1.1539 
1  .  1583 
1.1626 

1.0038 
1.0083 
1.0123  
1.0162 
1.0204 

(de  Coninck,  A.  ch.  1903,  (7)  28.  11.) 

1  pt.  is  sol.  in  8,  pts.  alcohol  (94°)  +Aq. 
(1:4)  at  10.4°.  (de  Coninck.) 

Solubility  in  glycol  at  14.8°  =  3.15%.  (de 
Coninck,  C.  C.  1905,  II.  883.) 

Min.  Johannite.    SI.  sol.  in  H2O. 

Uranous  hydrogen  sulphate,  U(SO4)2,  H2S04 

+  10H20. 
(Giolitti,  C.  C.  1905,  II.  1226.) 


SULPHATE,  VANADIUM 


1031 


Uranyl  sulphate,  basic,  3UO3,  SO8+2H2O. 

(Athanasesco.) 
+  14H2O.     Sol.   in   H2O.      (Ordway,   Sill. 
Am.  J.  (2)  26.  208.) 
4UO3,  SO3+7H2O.     (Athanasesco,  C.  E. 
103.  271.) 
UO2,  4UOSO4+8H2O.     Less  sol.  in  min. 
acids,  especially  dil.  H2SO4+Aq,  than  UOSO4 
+2H2O.    (de  Coninck,  C.  C.  1901,  II.  1038.) 

Sp.  gr.  of  (UO2)SO4+H2SO4(d  =  1.168)  at  t°. 
di  =  Sp.  gr.  referred  to  H2O. 
d2  =  Sp.  gr.  referred  to  H2SO4. 

t° 

%8alt    ' 

di 

d2 

20.6 
22.2 
21.1 
22.7 
22.3 

1 

2 
3 
4 
5 

.1738 
.1775 
.1880 
.1872 
.1918 

.0050 
.0082 
.0129 
.0165 
.0204 

+H2O.    (de  Coninck.) 

+3H2O.  Efflorescent.  Very  sol.  in  H2O 
and  alcohol. 

1  pt.  is  sol.  in  0.6  pt.  cold  H2O;  in  0.45 
•pt.  boiling  H2O;  in  25  pts.  cold  absolute 
alcohol;  in  20  pts.  boiling  absolute  alcohol. 
(Bucholz.) 

Sol.  in  0.47  pt.  H2O  at  21°,  and  0.28  pt. 
boiling  H2O.  (Ebelmen.) 

100  pts.  H2O  at  15.5°  dissolve  160  pts.,  and 
at  100°,  220  pts.  (Ure's  Diet.) 

1  pt.  is  sol.  in  5.3  pts.  H2O  at  13.2°;  5.16 


s.  at  14.1°;  4.96  pts.  at  15.1°;  4.88  pts.  at 
.5°.     (de  Coninck,  A.  ch.  1903,  (7)  28.  8.) 


Sp.  gr.  of  (UO2)SO4+Aq  at  t°. 


t° 

%  (UO)2S04 

Sp.  gr. 

14 

1 

1.0062 

15.5 

2 

1.0113 

11.3 

3 

1.0172 

10.2 

4 

1.0229 

10.2 

5 

1.0280 

10 

6 

.0338 

14 

7 

.0389 

15.6 

8 

.0442 

11 

9 

.0503 

10.3 

10 

.0557 

11.4 

11 

1.0612 

11.6 

12 

1.0669 

(de  Coninck,  A.  ch.  1903,  (7)  28.  7.) 


Solubility  in  acids  +Aq. 
1  pt.  (UO2)SO4  is  sol.  in: 
3.4  ts.  cone.  HC1  at  12.8 


"       "      "  13.6° 
HBr(d  =  1.21)  "     12.9° 
"     11.2° 

cone.  HNO3     "     12.3° 

"  "      "    10.8° 

H2SO4(d  =  l,38)"12.7° 


3.25 

5.9    " 

6.1     " 

10.8  " 

11.2" 

4.3   " 

4.1    "        "  "    "14.0° 

5.6  "  aqua  regia  (equal  vol.  HC1+  HNO3) 
at  15.4° 

5.47  pts.   aqua  regia   (equal  vol.  HC1+ 
HNO3)  at  16  4°. 

3.7  pts.  selenic  acid  (d  =  1.4)  at  15.3°. 

(de  Coninck,  A.  ch.  1903,  (7)  28.  8.) 


(de  Coninck,  A.  ch.  1903,  (7)  28.  I.) 

1  pt.  is  sol.  in  37.9  pts.  alcohol  (85°)  at 
16.7°;  38.6  pts.  at  15.8°.  (de  Coninck,  A. 
ch.  1903,  (7)  28.  8.) 

Very  si.  sol.  in  formic  and  glacial  acetic 
acids,  (de  Coninck,  A.  ch.  1903,  (7)  28.  9.) 

Completely  pptd.  from  (UO2)SO4+Aq  by 
HC2H3O2.  (Persoz.) 

Uranyl  hydrogen  sulphate,  (UO2)SO<,  H2SO<. 
Very  deliquescent.    (Schultz-Sellack.) 
2(UO2)SO4,  H2SO4+5H2O.    Very  deliques- 
cent.    (Wyrouboff,  Bull.  Soc.  Min.  1909,  32. 
351.) 

Uranyl  pyrosulphate,  (UO2)S2O7. 

Very  deliquescent.  Hisses  with  H2O. 
(Schultz-Sellack.) 


Uranouranyl  sulphate,  USO,,  (UO2)SO4. 

Sol.   in   H2O.      (Ebelmen.)      Decomp. 
boiling.     (Berzelius.) 

Min.  Voglianite. 


by 


Uranyl  sulphate  ammonia,  (UO2)SO4,  2NH8. 
(v.  Unruh,  Dissert.  1909.) 
(UO2)SO4,  3NH3.    (v.  Unruh.) 
(UO2)SO4,  4NH3.    (v.  Unruh.) 

Vanadous   sulphate,   V2O3,   4S03+9H2O. 
Sol.  in  H2O.     (Brierley,  Chem.  Soc.  49. 

882.) 

Vanadium  sulphate,  V2O6,  2SO3  =  (VO2)2S2O7. 

Deliquescent.    Easily  sol.  in  H2O. 

V2O6,  3SO3.  Deliquescent.  Sol.  in  H2O 
and  alcohol. 

+3H2O.  Deliquescent.  Very  sol.  in  H2O, 
but  decomp.  by  boiling.  Sol.  in  alcohol; 
(Ditte,  C.  R.  102.  757.) 

VSO4+7H2O.  Decomp.  by  air;  very  un- 
stable; sol.  in  H2O.  (Piccini,  Z.  anorg.  1899, 
19.  204.) 

Vanadium    sesgmsulphate,    V2(SO4)s. 

Anhydrous. 

Insol.  in  H2O. 

Insol.  in  cone.  H2SO4,  but  slowly  sol.  in 
boiling  dil.  H2SO4.  Sol.  in  HC1. 

Insol.  in  alcohol  and  ether.  (Stahler,  B. 
1905,  38.  3979.) 


1032 


SULPHATE,  ZINC,  BASIC 


Vanadium  hydrogen  sulphate, 
V2(SO4)3,  H2SO4+12H2O. 

Sol.  in  H2O. 

Sol.  in  HC1.  Insol.  jn  60%  H2SO4+Aq, 
alcohol,  ether  and  acetic  acid.  (Stahler,  B. 

1905,  38.  3978.) 

Divanadyl  sulphate,  V2O2(SO4)2. 

Insol.  in  H2O,  HC1,  or  H2SO4+Aq,  but 
on  heating  to  400°  becomes  sol.  in  H2O  if 
heated  to  130°  therewith.  (Gerland.) 

+4M2O.  Very  slowly  sol.  in  H2O  at  10°, 
quickly  at  60°,  and  still  more  rapidly  at  100°. 
Deliquesces  in  warm  moist  air  more  quickly 
than  it  dissolves  in  H2O  at  10°.  Insol.  in 
absolute  alcohol.  Very  sol.  in  alcohol  of  0.833 
sp.  gr.  (Berzelius.) 

+5H2O.  (Koppel  and  Behrendt,  Z. 
anorg.  1903,  36.  168.) 

+7H2O.andlOH2O. 

+  13H2O.    Efflorescent.    (Gerland.) 

2V2O4,  5SO3  +  18H2O.  (Gain,  C.  R.  1906, 
143.  1154.) 

V2O4,  3SO3  +  10H2O.  (G.) 

2V2O4,  7SO3+20H2O.  (G.) 

2V2O4,  9SO3+22H2O.  (G.) 

V2O4,  5SO3+12H2O.  (G.) 

Wtttt 

Divanadyl  hydrogen  sulphate, 

(V202)H2(S04)3  =  V204,   3S03+H20. 

+2H20. 

+3H2O.  Deliquescent.  Very  slowly  sol. 
in  cold  H2O  or  alcohol.  Easily  sol.  in  hot  H2O. 
(Gerland.) 

+5H2O.  Deliquescent.  Insol.  in  ether. 
Scarcely  sol.  in  alcohol.  Slowly  sol.  in  cold, 
easily  in  hot  H2O,  (Crow.) 

+  14H2O.  Easily  sol.  in  cold  H2O  or  dil. 
alcohol.  (Gerland.) 

2VO2,  3SO3.  SI.  sol.  in  H2O.  (Koppell 
and  Behrendt,  Z.  anorg.  1903,  35.  163.) 

2VOSO4,  H2SO4+H2O.  Very  slowly  sol. 
in  H2O.  (Koppel  and  Behrendt,  Z.  anorg. 
1903,  36.  163.) 

2VOSO4,  3H2SO4+15H2O.      (Gain,  C.  R. 

1906,  143.  1156.) 
2VOSO4,4H2SO4+16H2O.  (G.) 
2VOSO4,  5H2SO4+15H2O.  (G.) 
2VOSO4,  7H2SO4+15H2O.  (G.) 
2VOSO4,  8H2SO4  +  16H2O.  (G.) 

Ytterbium  sulphate,  Yb2(SO4)3+8H2O. 

Quite  slowly  sol.  in  H2O  even  at  100°. 
Anhydrous  salt  is  easily  sol.  in  much  H2O, 
but  if  little  H2O  is  used  the  hydrous  salt  is 
formed,  which  only  slowly  dissolves.  Sol. 
in  K2SO4+Aq. 

100  pts.  H2O  dissolve  at: 
0°  15.5°  35°  55°  60° 
44.2  34.6  19.1  11.5  10.4  pts.  Yb2(SO4)3, 

70°       80°       90°       100° 

7.22     6.93    5.83    4.67  pts.  Yb2(SO4)3. 

(Cleve,  Z.  anorg.  1902,  32.  143.) 


Yttrium  sulphate,  basic,  Y2O3,  SO3  = 

(YO)2S04. 

Insol.  in  H2O.    (Berzelius.) 
2Y2O3,  SO3+10H2O.     (Cleve.) 

Yttrium  sulphate,  Y2(SO4)3. 

Anhydrous.  More  sol.  in  H2O  than  the 
hydrous  salt,  and  more  sol.  in  cold  than  hot 
H2O.  Solution  sat.  at  0°  separates  Y2(SO4)3+ 
8H2O  at  50°.  100  pts.  H2O  dissolve  15.2  pts. 
anhydrous  salt,  at  ord.  temp. 

5.38  pts.  are  sol.  in  100  pts.  H2O  at  25°. 
(James  and  Holden,  J.  Am.  Chem.  Soc.  1913, 
35.  561.) 

Easily  sol.  in  large  amount  of  sat.  K2SO4  + 
Aq,  from  which  3K2SO4,  2Y(SO4)3  is  pptd.  on 
warming.  (Cleve  and  Hoglund,  Sv.  V.  A. 
H.  Bih.  1.  No.  8.) 

Solubility  of  Y2(SO4)3  in  Na2SO4+Aq  at  25° 


Pts. 

Y2(S04)3 

per  100 
pts.  H2O 

Pts. 
Na2S04 
per  100 
pts.  H20 

Solid  phase 

5.61 

1.29 

6.38 
7.40 

3.85 

6.21 

Y2(S04)3 

8.43 

8.53 

5.86 

7.57 

4.75 

7.72 

3.42 

10.14 

2.36 

11.36 

-   2.02 

13.42 

1.90 

14.89 

1.79 
1.86 

16.51 
18.44 

Y2(SO4)3,Na2SO4+2H2O 

2.99 

19.96 

3.04 

21.05 

2.27 

27.14 

1.52 

28.22 

1.61 

28.13 

5.38 

0.0 

Na2S04-flOH2O 

(James  and  Holden,  J.  Am.  Chem.  Soc.  1913, 
36.  560.) 

+8H2O.  100  pts.  H2O  dissolve  9.3  pts.  of 
cryst.  salt  at  ord.  temp.,  and  4.8  pts.  at  100°. 
(Cleve,  Bull.  Soc.  (2)  21.  .344.) 

Less  sol.  in  H2O  containing  H2SO4  than  in 
pure  H2O.  (Berzelius.) 

Completely  pptd.  by  HC2H3O2+Aq.  In- 
sol. in  alcohol. 

Yttrium  hydrogen  sulphate,  Y2(SO4H)3. 
(Brauner,  Z.  anorg.  1904,  38.  332.) 

Zinc  sulphate,  basic,  8ZnO,  SO3+2H2O. 

Insol.  in  H2O.  (Schindler,  Mag.  Pharm. 
31.  181.) 

6ZnO,SO3+10H2O.  Insol.  in  H2O.  (Kane, 
A.  ch.  72.  310.) 

4ZnO,  SO3+2H2O.  Scarcely  sol.  in  hot 
or  cold  H2O.  Sol.  in  ZnSO4+Aq.  (Kiihn, 
Schw.  J.  60.  337.) 


SULPHATE,  ZINC,  BASIC 


1033 


+3H2O.    (Werner,  B.  1907,  40.  4443.) 

Solubility  of  ZnSO4  in  100  pts.  H2O  at  t°. 

+5H2O.    Nearly  insol.   in  H2O.     (Haber- 

mann,  M.  6.  432.) 

Pts 

Pts 

Pts. 

+6H2O.     (Kraut,  Z.  anorg.  1897,  13.  5.) 

+  *TTT  r\          /  A  j.l~                                /~i      T>        -i  r\'t       r>Ti    \ 

t° 

ZnS04 

t° 

ZnS04 

t 

ZnSO< 

7H2(J.     (Athanasesco,  C.  R.  103.  271.) 
-f-8H2O.     Extremely    slowly    decomp.  bv 
H2O.     (Reindel,  J.  pr.  1869,  (1)  106.  373.') 

0 
1 

44.0 
44.6 

14 

15 

52.8 
53.5 

'27 
28 

62.1 

62.8 

+  10H2O.     (Schindler.) 

2 

45.2 

16 

54.2 

•  29 

63.6 

3ZnO,  SO3.     Insol.  in  cold,  si.  sol.  in  hot 

.3 

45.8 

17 

54.9 

30 

64.3 

H20.     (Vogel.) 

4 

46.4 

18 

55.6 

31 

65.1 

2ZnO,  SO3.     (Athanasesco.) 

5 

47.0 

19 

56.3 

32 

65.8 

5ZnO,  SO3.    (Pickering,  Chem.  Soc.  1907, 

6 

47.6 

20 

57.0 

33 

66.6 

91.  1986.) 

7 

48.3 

21 

57.7 

34 

67.3 

+4H2O.      (Moody,  Am.  J.  Sci.  1906,   [4] 

8 

48.9 

22 

58.4 

35 

68.1 

22.   184.) 

9 

49.5 

23 

59.2 

36 

78.8 

9ZnO,  2SO3  +  12H2O.    (Reindel,  J.  pr.  1869, 

10 

50.2 

24 

59.9 

37 

69.3 

(1)  106.  374.) 

11 

50.8 

25 

60.7 

38 

70.4 

Zinc  sulphate,  ZnSO4. 
Sol.  in  HoO  with  evolution  of  heat. 

12 
13 

51.5 
52.2 

26 

61.4- 

39 

71.2 

Sol.  in  HCl+Aq. 

+H2O.     (Etard.) 

+2H2O.     Insol.  in  alcohol.     (Kuhn.) 

+33^H2O.     (Anthon.) 

+5H2O.  Insol.  in  boiling  alcohol  of  0.86 
sp.  gr.  (Kuhn.) 

+6H2O.     (Marignac.) 

+7H2O.    Slowly  efflorescent. 

M.-pt.  of  ZnSO4+7H2O=50°.  (Tilden, 
Chem.  Soc.  45.  409.) 

For  solubility  data  on  hydrated  salts,  see 
below. 

Sol.  in  2  +  pts.  H2O  at  ord.  temp.,  and  in  less  at  100°. 
(Bergmann.) 

100  pts.  H2O  at  104.4°  dissolve  81.81  pts.  ZnSO*. 
(Griffiths.) 

100  pts.  H2O  at  ord.  temp,  dissolve  140  pts.  ZnSO4  + 
7H2O.  (Dumas.) 

Sol.  in  2.29  pts.  H2O  at  18.75°.     (Abl.) 

100  pts.H2O  at  15.56°  dissolve  140  pts.  ZnSO4+7H2O. 
Ure's  Diet.) 

100  pts.  H2O  at  15°  dissolve  140.53  pts.  ZnSO4  + 
7H2O,  and  has  sp.  gr.  =1.4442.  (Michel  and  Krafft.) 

1  pt.  of  the  crystals  dissolves  in  0.923  pt. 
H2O  at  17.5°,  and  forms  a  solution  of  1.4353 
sp.  gr.  (Karsten.) 

100  pts.  ZnSO4+Aq  sat.  at  18-20°  contain 
35.36  pts.  ZnSO4.  (v.  Hauer,  J.  B.  1866.  59.) 

100  pts.  H2O  dissolve  at: 
0°  20°  50°  75 

41.3         53.0         66.9         80.4  pts.  ZnSO4. 
(Tobler,  J.  B.  1865.  309.) 

100  pts.  H2O  at  20.5°  dissolve  163.2  pts. 
ZnSO4+7H2O.  (Schiff,  A.  109.  336.) 

100  pts.  H2O  at  t°  dissolve  pts.  anhydrous 
ZnSO4,  and  pts.  ZnSO4+7H2O. 


t° 

Pts. 
ZnSO4 

Pts. 
ZnSO4  + 
7H20 

t° 

Pts. 
ZnS04 

Pts. 
ZnSO4  + 
7H2O 

0 

43.02 

115.22 

60 

74.20 

313.48 

10 

48.36 

138.21 

70 

79.25 

369.36 

20 

53.13 

161.49 

80 

84.60 

442.62 

30 

58.40 

190.90 

90 

89.78 

533.02 

40 

63.52 

224.05 

100 

95.03 

653.59 

50 

68.75 

263.84 

...' 

(Poggiale,  A.  ch.  (3)  8.  467.) 


Decomp.  into  basic  salt  above  40°. 
(Mulder,  Scheik.  Verhandel.  1864.  74.) 


If  solubility  S  represents  number  of  pts. 
anhydrous  salt  in  100  pts.  of  solution,  S  = 
27.6+0.2604t  from  —5°  to  +81°;  S  =  50.0— 
0.2244t  from  81°  to  175°.  (fitard,  C.  R.  106. 
207.) 

Sat.  ZnSO4+Aq  contains  at: 
1°        13°      20°      41°      49° 
29.1   32.6  34.8  40.2   40.9%ZnSO4, 

55°     62°     70°      77°      100° 

43.4  45.0  47.0   46.5  44.7%ZnSO4, 

111°    12.°    137°    144°    169°    171° 

43.0  40.7  38.0  37.4   30.0  29.0%ZnSO4. 

(fitard,  A.  ch.  1894,  (7)  2.  551.) 


Transition  point  from  +6H2O  to  +1H2O 
is  70°.    (fitard.) 


Solubility  of  ZnSO4+6H2O  in  H2O  at  t°. 


t° 

g.  ZnS04  in  100  g.  H2O 

—5.0 

47.08 

+0.1 

49.48 

9.1 

54.20 

15.0 

57.15 

25.0 

63.74 

30.0 

65.82 

35.0 

67.99 

39.0 

70.08 

(Cohen,  Z.  phys.  Ch.  1900,  34.  182.) 

1034 


SULPHATE,  ZINC,  BASIC 


Solubility  of  the  hepta-and  hexa-hydrates  of 

ZnSO4  at  t°. 

p=wt.  of  salt  expressed  in  percent  of  solu- 
tion. 


Sat.  ZnSO4+Aq  at  8°  has  sp.  gr.  =  1.421, 
(Anthon.) 


t° 

P 

Sp.  gr.  of  ZnSO4+7H2O  at  20.5°. 
•    %  =  %ZnS04+7H20. 

0       ' 
0 
0 
15.00 
15.88 
30.70 
39.92 
39.95 
40.73 
41.49 
46.40 
49.97 
49.99 
50.00 
50.02 

29.43 
29.53 
29.49 
33.66 
33.85 
38.46 
41.36 
41.37 
41.43 
41.70 
42.68 
43.51 
43.41 
43.50 
43.51 

% 

Sp.  gr. 

% 

Sp.  gr. 

% 

Sp.  gr. 

1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 

1.0057 
1.0115 
.0173 
.0231 
.0289 
.0348 
.0407 
.0467 
.0527 
.0588 
.0649 
.0710 
.0772 
.0835 
1,0899 
1.0962 
1  .  1026 
1.1091 
1.1156 
1  .  1222 

21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
34 
35 
36 
37 
38 
39 
40 

1  .  1288 
1  .  1355 
1  .  1423 
1  .  1491 
1  .  1560 
1  .  1629 
1  .  1699 
1.1770 
1  .  1842 
1.1914 
1  .  1987 
1  .  2060 
1.2134 
1.2209 
1.2285 
1.2362 
1.2439 
1.2517 
1.2595 
1.2674 

41 
42 
43 
44 
45 
46 
47 
48 
49 
50 
51 
52 
53 
54 
55 
56 
57 
58 
59 
60 

1.2754 
1.2834 
1.2917 
1.3000 
.3083 
.3167 
.3252 
.3338 
.3424 
.3511 
.3599 
.3688 
.3779 
.3871 
.3964 
1.4057 
1.4151 
1  .  4246 
1.4342 
1.4439 

Transition  point  from  +7H2O  to  +6H2O 
is  39°. 
The  formula  representing   the   change  of 
solubility  between  0°  and  39°  is 
p  =  29  .  5  +0  .  270t  +0  .  00068t2 
while    the    expression    for    the    hexahydrate 
above  40°  is 
p=41.35+0.210t+0.00070t2. 
(Barnes,  J.  phys.  Chem.  1900,  4.  19.) 

Solubility  of  ZnSO4+7H2O  in  H2O  at  t°. 

(Schiff,  A.  110.  72.) 

Sp.  gr.  of  ZnSO4+Aq  at  15°. 
%  =  %ZnS04+7H20. 

t° 

g.  ZnSO4  in  100  g.  H2O 

—5 
+0.1 
9.1 
15.0 
25.0 
35.0 
39.0 

39.30 
41.93 
47.09 
50.88 
57.90 
66.61 
70.05 

% 

Sp.  gr. 

% 

Sp.  gr. 

% 

Sp.  gr. 

1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 

.006 
.013 
.019 
.024 
.0288 
.035 
.041 
.047 
.053 
.0593 
.066 
1.073 
1.079 
1.085 
.0905 
.097 
.103 
.110 
.116 

.1236 

• 

21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
34 
35 
36 
.37 
38 
39 
40 

1.130 
1.137 
1.143 
.150 
.1574 
.164 
.171 
.179 
1.185 
1  .  1933 
1.200 
1.209 
1.216 
1.224 
1.231 
1.240 
1.246 
1.255 
1.263 
1.2709 

41 
42 
43 
44 
45 
46 
47 
48 
49 
50 
51 
52 
53 
54 
55 
56 
57 
58 
59 
60 

1.280 
1.288 
1.295 
1.304 
1.3100 
1.320 
1.330 
1.337 
1.346 
1.3532 
1.362 
1.380 
1.370 
1.390 
1  .  3986 
1.408 
1.416 
1.425 
1.435 
1.4451 

(Cohen,  Z.  phys.  Ch.  1900,  34.  182.) 
Solubility  in  H2O  at  high  pressures: 

Pressure                .  0 
in  atm. 

g.  ZnSO4  in 
100  g.  H2O 

Solubility 
at  25° 

1           26 
500           26 

500           25.8 
1000           25.8 
1000           25.8 

57.95 
58.43 
58.32 
57.95 
57.95 

57.95 
57.92 
57.91 
57.55 
57.55 

(Cohen  and  Sinnige,  Z.  phys.  Ch.  1909,  67. 

444.) 

Liable  to  form  supersaturated  solutions. 

(Gerlach,  Z.  anal.  8.  288.) 

SULPHATE,  ZINC,  BASIC 


1035 


Sp.  gr.  of  ZnSO4+A 
equivalent  to  } 
1000  g.  H2O;b 
7H2O,  Yi  mol.  \ 
is  ZnSO4,  Y>.  me 

q  at  2c 
4  mol. 
=  sp.  gi 

1.5°.    a  =  no.  of  g., 
wt.,  dissolved  in 
.  if  a  is  ZnSO4  + 
3.5;  c  =  sp.  gr.  if  a 
=80.5. 

Sp.  gr.  of 

ZnSO4+Aq. 

g.  salt  in  100  g.  solution 

Sp.  gr. 

vt.  =  14 
1.  wt.  = 

24.7170 
21.4444 
17.7573 
14.0307 
9.7426 
5.1110 

1.3152 
1.2665 
1.2145 
1  .  1645 
1.1106 
1.0565 

a 

b 

c 

a 

b 

1 
2 
3 
4 
5 
6 

1.077 
1.143 
1.199 
1.249 
1.294 
1.333 

.084 
.162 
.236 
.307 
.376 
.443 

7 
8 
9 
10 
11 

1.368 
1.400 
1.428 
1.453 
1.476 

(Charpy,  A.  ch.  1893,  (6)  29.  27.) 
Sp.  gr.  of  ZnSO4+Aq. 

(Favre  and  Valson,  C.  K 
Sp.  gr.  of  ZnSO4+Aq 

.  79.  968.) 
at  18°. 

g.  equivalents 
ZnSO4  per  liter 

•    t 

0 

Sp.  gr.  t°/t° 

0.001309 
0.002616 
0.005212 
0.01039 
0.09818 
0.18842 
0.1890 
2.493 

13.59 
13.575 
13.573 
13.585 
13.621 
13.642 
16.11 
15.88 

.0001126 
.0002258 
.0004451 
.000886 
.008189 
.015587 
.01550 
.  19385 

o 
1 

N 
tf 

5 

10 

Sp.  gr. 

N 
&§ 

Sp.  gr. 

1 

N 
£§ 

Sp.  gr. 

1.0509 
1  .  1369 

15 
20 

1  .  1675 
1.2313 

32 
50 

1.3045 

1.3788 

(Kohlrausch  and  Hallwachs,  W.  Ann.  1894, 
63.  27.) 

(Kohlrausch,  W.  Ann.  1879.  1.) 

Sp.  gr.  of  ZnSO4+Aq  at  room  temp,  con 
taining  : 

7.12  16.64       23.09%ZnSO4. 

1.1064       1.1953       1.2814 


Sp.  gr.  of  ZnSO4+Aq  at  18.5°,  when  p  = 
percent  strength  of  solution;  d=  ob- 
served density;  and  w  =  volume  cone. 


in  grams  per  cc. 


(Wagner,  W.  Ann.  1883,  18.  271.) 
Sp.  gr.  of  ZnS04+Aq  at  19.5°. 

p 

d 

W 

29.22 
25.14 
21.28 
17.08 
11.20 
8.44 
6.65 
3.82 
3.18 
1.46 
0.577 

1.3718 
1.3091 
1.2528 
1  .  1957 
1  .  1220 
1.0894 
1.0696 
1.0387 
1.0318 
1.0138 
1.0045 

0.40057 
0.32910 
0.26659 
0.20422 
0.12567 
0.09195 
0.07112 
0.03968 
0.03281 
0.01480 
0.00580 

Mass  of  salt  per  unit 
mass  of  solution 

Density  of  solution. 
(g.  per  cc.) 

0.00186 
0.00371 
0.00556 
0.00740 
0.01106 
0.01469 
0.01829 
0.02187 
0.02542 
0.02895 

.00179 
.00356 
.00530 
.00711 
.01065 
.01410 
.01753 
.02112 
.02446 
1.02798 

(Barnes,  J.  phys.  Chem.  1898,  2.  542.) 

Sp.  gr.  of  dil.  ZnSO4+Aq  at  20.004°. 
Cone.  =g.  equiv.  per  1.  at  20.004°. 
Sp.  gr.  compared  with  H2O  at  20.004°  =  1  • 

(McGregor,  C.  N.  1887,  65.  4.) 
Sp.  gr.  of  ZnSO4+Aq  at  25°. 

Cone. 

Sp.  gr. 

0.0000 
0.0001 
0.0002 
0.0005 
0.0010 
0.0020 
0.0050 
0.0060 
1.0100 

1.000,000,0 
1.000,008,6 
1.000,017,2 
1.000,043,2 
1.000,086,3 
1.000,172,3 
1.000,429,1 
1.000,514,3 
1.000,853,9 

Concentration  of  ZnSCh 
+Aq 

Sp.  gr. 

1  —  normal 

i  /  (t 

1.0792 
1.0402 
1.0198 
1.0094 
1.0047 

(Lamb  and  Lee,  J.  Am.  Chem.  Soc.  1913,  35. 
1690.) 

(Wagner,  Z.  phys.  Ch.  1890,  5.  40.) 

1036 


SULPHATE,  ZINC  HYDROGEN 


Sat.  ZnSO4+Aq  boils  at  104.4°,  and  solu- 
tion contains  45  pts.  ZnSO4  to  100  pts.  H2O. 
(Griffiths.) 

Crust  forms  at  103.5°,  the  solution  contain- 
ing 68  pts.  ZnSO4  to  100  pts.  H2O.  Highest 
temp,  observed,  105°.  (Gerlach,  Z.  anal.  26. 
426.) 

B.-pt.  of  ZnSO4+Aq  containing  pts.  ZnSO4 
to  100  pts.  H2O. 


B.-pt. 

Pts.  ZnSO4 

B.-pt.          Pts.  ZnSO4 

100.5° 

13.1 

103.0°          61.0 

101.0 

25.0 

103.5            68.0 

101.5 

37.7 

104.0            74.9 

102.0 

45.4 

104.5            80.7 

102.5 

53.9 

105.0            85.7 

(Gerlach,  Z.  anal.  26  432.) 

B.-pt.  of  ZnSO4+Aq. 

g.  ZnS04 

in 

Rise 

of  the 

Barometric 

100  g.  H20 

b. 

-pt. 

pressure  mm. 

2.886 

0. 

080 

743.0 

6.647 

0. 

169 

10.139 

0. 

266 

13.389 

0. 

372 

17.713 

0. 

461 

22.202 

0. 

591 

25.199 

0. 

690 

28.249 

0. 

811 

30.470 

0. 

899 

742.0 

32.89 

0. 

995 

35.18 

1. 

122 

37.36 

1. 

240 

39.83 

1. 

381 

41.30 

1. 

459 

44.56 

1. 

671 

(Kahlenberg,  J.  phys.  Chem.  1901,  6.  370.) 

1  1.  absolute  H2SO4  dissolves  0.0021  mols. 
ZnSO4  at  25°.  (Bergius,  Z.  phys.  Ch.  1912, 
72.  353.) 

Completely  pptd.  from  ZnSO4+Aq  by 
HC2H3O2.  (Persoz.) 

Solubility  of  ZnSO4  in  KOH+Aq. 


Mols.  KOH  to  1  mol. 
ZnSO4 

per  cent  ZnO  in  ppt. 

,0.25 
0.50 
1.00 
1.62 
2.00 
3.00 
5.00 
7.00 
13.20 

17.11 
35.10 

68.08 
100.00 
98.49 
96.79 
89.76 
68.87 
0.00 

(Linebarger,   J.   Am.   Chem.  Soc.   1895,   17. 
360.) 

Difficultly  and  slowly  sol.  in  sat.  NH4C1  + 
Aq,  with  separation  of  a  double  sulphate. 

Sol.  in  considerable  quantity  in  sat.  NaCl 
+Aq,  without  pptn.  at  first,  but  finally 
Na2SO4  separates  out.  See  under  NaCl. 

Sol.  in  sat.  NaNO3+Aq  as  in  NaCl+Aq. 
See  under  NaNO3. 

Sol.  in  sat.  KNO3+Aq  with  immediate 
pptn.  of  double  sulphate.  (Karsten.)  See 
under  KNO3. 

Very  rapidly  sol.  in  sat.  K2SO4+Aq,  with 
separation  of  a  double  salt.  (Karsten.)  See 
under  K2SO4. 

Abundantly,  in  sat.  CuSO4+Aq. 

Slowly  sol.  in  sat.  MgSO4+Aq. 

Very  rapidly  and  abundantly  sol.  in  sat. 
NaSO4+Aq. 

For  solubility  of  ZnSO4+Na2SO4  see  under 
Na2SO4  and  Na2Zn(SO4)2+4H2O. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  830.) 

Insol.  in  alcohol  of  0.88  sp.  gr.  ;  1000  pts. 
alcohol  of  0.905  sp.  gr.  dissolve  2  pts. 
(Anthon.) 

100  pts.  of  a  saturated  solution  in  40% 
alcohol  contain  3.48  pts.  ZnSO4+7H2O;  20%, 
39  pts.;  10%,  51.1  pts.  (Schiff,  J.  B.  1861. 
87.) 

100  pts.  absolute  methyl  alcohol  dissolve 
0.65  pt.  ZnSO4  at  18°.  (de  Bruyn,  Z.  phys. 
Ch.  10.  783.) 

100  pts.  absolute  methyl  alcohol  dissolve 
59  pts.  ZnSO4+7H2O  at  17°. 

100  pts.  50%  methyl  alcohol  dissolve  15.7 
pts.  ZnSO4+7H2O  at  17°.  (de  Bruyn.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329.) 

100  pts.  glycerine  dissolve  35  pts.  ZnSO4 
at  ord.  temp.  (Klever,  Bull.  Soc.  1872,  (2) 
18.  372.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790);  ethvl  acetate.  (Naumann, 
B.  1904,  37.  3601.) 

Min.  Gosslarite. 

Zinc  hydrogen  sulphate,  ZnH2(SO4)2+8H2O. 
Somewhat  difficultly  sol.  in  cold,  easily  in 
hot  H2O.    (v.  KobeU,  J.  pr.  28.  492.) 

Zinc  sulphate  ammonia,  basic.  4NH3.  4ZnO. 
S03+4H20. 

Ppt.     (Schindler.) 
Zinc  sulphate  ammonia,  ZnSO4,  2NH3. 

+H2O.  Decomp.  by  H2O  into  basic  zinc 
sulphate. 

ZnSO4,  4NH3+4H2O.  Sol.  in  H2O.  (Kane, 
A.  ch.  72.  304.) 

+3H2O.    (Andre,  C.  R.  100.  241.) 

ZnSO4,  5NH3.  Sol.  in  H2O  with  partial 
decomp.  (Rose,  Pogg.  20.  149.) 

Zinc  sulphate  cupric  oxide,  ZnSO,,  2CuO-f 

5H2O. 

(Mailhe,  A.  ch.  1902,  (7)  27.  169.) 
ZnSO4,    3CuO+sH2O.       (Recoura,    C.  R. 

1901,  132.  1415.) 


SULPHURIC  VANADIC  ACID                                         1037 

+5H20. 
2ZnSO4,  3CuO  +  12H2O.      (Mailhe,  A.  ch. 

Solubility   of   Zr(SO4)2-f-4H2O    in    H2SO4+ 
Aq  at  t°.  —  Continued, 

1902,  (7)  27.  169.) 

• 

7ZnS04,  24Cu6+zH2O.      (Recoura,  C.  R. 

1  rw"v~l       •!  oo      i  A  1  er   \ 

t° 

g.  ZrO2 

g.  S03 

1901,  132.  1415.) 

0.33 

42.1 

Zinc  sulphate  hydrazine,  ZnSO4,  2N2H4. 

0.14 

46.8 

Sol.  in  NH4OH+Aq.     (Franzen,  Z.  anorg. 
1908,  60.  278.) 

0.13 
0.15 

47.1 
56.7 

Sol.    in    NH4OH+Aq    without    decomp. 
(Curtius,  J.  pr.  1894,  (2)  60.  345.) 
ZnH2(SO4)2,  N2H4.  -    1  pt.  is  sol.  in  185  pts. 
H2O  at  12°.    SI.  sol.  in  dil.  acids.     Decomp. 
by   cone.   HNO3  and  by    hot    cone.    H2SO4. 
Very    sol.    in    NH4OH+Aq.      (Curtius,    J. 
pr.  1894,  (2)  50.  331.) 

0.20 
0.27 
0.50 
0.60 
2.00 
3.25 
4.40 

56.8 
57.1 
57.5 
57.8 
59.5 
60.4 
61.4 

Zirconium  sulphate,  basic,  3ZrO2,  2SO3. 

22, 

0.10 
0.13 

56.1 
46  ^ 

Insol.  in  H2O.     Sol.  in  HCl+Aq.     (Pay- 

0*21 

rrU  .  O 

57.2 

kull,  B.  12.  1719.) 

4ZrO2,  3SO3+14H2O.  Ppt.  Difficulty  sol. 
in  H2O.  (Hauser,  B.  1904,  37.  2024.) 

3ZrO2,  SO3.  Insol.  in  boiling  H2O.  (Franz, 
B.  3.  58.) 

7ZrO2,  6SO3.  Insol.  in  H2O.  (Endemann, 
J.  pr.  (2)  11.  219.) 

ZrO2,  SO 3.  Sol.  in  very  little  H2O.  More 
H2O  decomp.  into  3ZrO2,  2SO3  and  Zr(SO4)2. 
(Berzelius.) 

3ZrO2,  4SO3  +  15H2O.  Sol.  in  H2O.  (Pay- 
kull.)- 

6ZrO2,  7SO3  +  19H2O.  Sol.  in  H2O.  (Pay- 
kull.) 


(Hauser,  Z.  anorg.  1907,  64.  197.) 

Zirconium   hydrogen    sulphate,    Zr(S04)2, 
H2SO4+H20. 

Solubility  in  H2SO4+Aq.  at  39.5°. 

100  g.  of  the  solution  contain: 

0.11         0.10        0.10        g.  ZrO2 
81.4        81.6        81.5        g.  S03. 

(Hauser,  Z.  anorg.  1907,  54.  200.) 

+3H2O. 

Solubility  in  H2SO4+Aq  at  t°. 


Zirconium  sulphate,  Zr(SO4)2. 

100  g.  of  the  solution  contain: 

Anhydrous.      Slowly    but    completely    sol. 

t 

g.  ZrOa 

g.  S03 

Sol.  in  warm  H2SC>4,  but  separates  on  cool- 

39.5 

4.55 

61.5 

ing.     Precipitated  from  aqueous  solution  by 

3.25 

62.5 

alcohol. 

3.33 

63.8 

+4H2O.    Easily  sol.  in  H2O. 

3.35 

63.8 

100  pts.  of  the  solution  contain  59.3  pts. 

1.80 

64.2- 

of  the  hydrated  salt  at  39.5°.     (Hauser,  B. 

1.60 

64.6 

1904,  37.  2025. 

1.55 

65.0 

1.12 

66.8 

Solubility   of    Zr(SO4)2+4H2O    in   H2SO4+ 

0.96 

68.4 

Aq  at  t°. 
100  g.  of  the  solution  contain: 

22 

0.80 

66.4 

0.65 

67.5 

t° 

g.  ZrO2 

g.  S03 

0.60 

68.1 

39.5 

19.5 

25.46 

(Hauser,  Z.  anorg.  1907,  64.  200.) 

19.3 

25.6 

19.6 

25.99 

Fersulphuric  acid,  HSO4 

19.3 

18.8 

26.5 
27.0 

See  Persulphuric  acid. 

18.15 
17.3 

27.6 
25.3 

Pt/rosulphuric  acid  and  pT/rosulphates. 

16.2 

29.1 

See  under  Sulphuric  acid  and  sulphates. 

9.6      - 

32.3 

5.3 

34.7 

Sulphuric  boric  acid. 

3.51 
1.03 

36.01 
38.2 

See  Borosulphuric  acid. 

0.46 

001 

39.8 

49  0 

Sulphuric  vanadic  acid,  V2O6,  3SO8+3H02. 

.  O  -I- 

^.£  .  \J 

See  Sulphate,  vanadium. 

1038 


SULPHUROUS  ACID,  ANHYDROUS 


Sulphurous  acid,  anhydrous,  SO2. 
See  Sulphur  efo'oxide. 

Sulphurous  acid,  H2SO3. 

Known  only  in  aqueous  solution,  from 
which  SO 2  is  given  off  upon  heating.  Crys- 
tallizes in  cold,  with  various  amounts  of 
water,  forming  compounds  which  approxi- 
mate H2SO3+8H2O  (Pierre,  A.  68.  228); 
H2SO3+10H2O  (Dopping,  Bull.  Ac.  St. 
Petersb.  7.  100);  H2SO3  +  14H2O  (Schon- 
feld,  A.  95.  22);  H2SO3+6H2O  (Roozeboom, 
R.  t.  c.  3.  29,  59,  75,  84;  Geuther,  A.  224. 
218).  Crystals  are  sol.  in  2  pts.  H2O  at  10°. 
(Pierre.) 

For  sp.  gr.  of  solutions,  etc.,  see  sulphur 
dioxide. 

Sulphites. 

Normal.  Only  the  alkali  sulphites  are  sol. 
in  H2O,  and  they  are  insol.  or  only  si.  sol.  in 
alcohol. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  ch. 
J.  1898,  20.  824.) 

Acid.    All  the  acid  sulphites  are  sol.  in  H2O. 

In  general  it  is  rarely  possible  to  determine 
whether  the  compd.  described  is  a  pure 
chemical  compound  or  not.  It  is  probable 
that  many  substances  described  by  Svenssen 
and  others  are  isomorphic  mixtures  whose 
composition  depends  upon  the  temp,  and 
cone,  of  the  solution  in  which  it  was  pptd. 
(Rosenheim,  Z.  anorg.  1900,  25.  72.) 

Aluminum  sulphite,  basic,  A12O3,  SO2-f  4H2O. 

Insol.  in  H2O;  sol.  in  H2SO3+Aq.  (Four- 
croy  and  Vauquelin.) 

6A1(OH)3,A12(SO3)3+9H2O.  Ppt.  (Seubert, 
Z.  anorg.  1893,  4.  66.) 

Ammonium  sulphite,  basic,  (NH4)2SO3,  NH3 
•+3/2H20. 

Sol.  in  H2O.  Pptd.  from  aqueous  solution 
by  alcohol.  (Muspratt.) 

Does  not  exist.     (Marignac.) 

Ammonium  sulphite,  (NH4)2SOs. 

Very  hydroscopic.  (Divers,  Chem.  Soc. 
1900,  77.  336.) 

Insol.  in  acetone.  (Eidmann,  C.C.  1899, 
II.  1014.) 

+H2O.  Slowly  sol.  in  H^O.  (Muspratt, 
A.  50.  268.) 

Sol.  in  1  pt.  H2O  at  12°.  (Fourcroy  and 
Vauquelin,  Crell.  Ann.  1800.  2.  415.) 

More  sol.  in  hot  H2O  with  evolution  of 
NH3.  SI.  sol.  in  absolute  alcohol.  (Mus- 
pratt.) , 

Much  more  sol.  in  alcohol  than  K2SO3. 
(Pierre.) 

Loses  NH3  in  the  air. 

Sol.  in  H2O.  Cone,  solution  charged  with 
NH3  will  deposit  salt  on  evaporation  over 
KOH.  Dil.  solution  decomp.  on  evaporation. 
(Divers,  Chem.  Soc.  1900,  77.  335.)- 


Insol.   in   acetone. 
37.  4329.) 


(Naumann,    B.    1904, 


Ammonium   hydrogen   sulphite,    NH4HSO3. 

Insol.  in  acetone.      (Eidmann,  C.C.  1899, 

II.    1014;     Naumann,  B.   1904,    37.    4329.) 

Ammonium    p?/rosulphite,    (NH4)2S2O5. 

Deliquescent.  Very  sol.  in  H2O  and 
alcohol.  Insol.  in  ether.  (Fock  and  Kliiss, 
B.  23.  3149.) 

Very  sol.  in  H2O;  very  hydroscopic.  Aq. 
solution  is  si.  decomp.  on  evaporation. 
(Divers,  Chem.  Soc.  1900,  77.  336.) 

Ammonium  cadmium  sulphite,   (NH4)2SO3, 

CdSO3. 

Nearly  insol.  in  H2C.  Partly  sol.  in  excess 
of  H2SO3+Aq,  but  separates  out  on  boiling. 
(Schuler,  A.  87.  34.) 

Ammonium  cobaltous  sulphite,   (NH4)2SO3, 

CoSO3+o;H2O. 
Decomp.  on  air.     (Berglund,  B.  7.  469.) 

Ammonium  cobaltocobaltic  sulphite. 
See  Cobaltisulphite,  ammonium  cobalt. 

Ammonium  cuprous  sulphite,  (NH4)2SO3, 
2Cu2SO3+2H20. 

(Bottinger,  A.  51.  411.) 

(NH4)2SO3,  Cu2SO3.  Insol.  in  cold,  de- 
comp. by  boiling  H2O.  (Rogojski,  J.  B.  1851. 
366.) 

Decomp.  by  warming  with  H2O,  in  which 
it  is  insol.  Sol.  in  acids  with  evolution  of 
SO2.  (Rosenheim  and  Steinhauser, 'Z.  anorg. 
1900,  25.  99.) 

+2H2O.      (Commaille,   J.   B.   1867.   300.) 

2(NH4)2SO3,  Cu2SO3+3H2O.  Very  sol.  in 
H2O.  Solution  decomp.  on  standing.  De- 
comp. by  acids.  (Rosenheim  and  Stein- 
hauser.) 

5(NH4)2SO3,  Cu2SO3+2H2O.  Decomp. 
on  air.  Sol.  in  H2O  with  decomp.  (Svensson.) 

6(NH4)2SO3,  Cu2SO3+4H2O.  Easily  de- 
comp. (Rosenheim  and  Steinhauser.) 

7(NH4)2SQ3,  Cu2SO3+4H2O.  Very  sol.  in 
H2O.  Solution  soon  decomp.  (Rosenheim 
and  Steinhauser.) 

+  10H2O.  Decomp.  on  air.  81.  sol.  in 
warm,  less  sol.  in  cold  H2O.(de  Saint-Gilles.) 

-)-14H2O.  Decomp.  on  air.  Sol.  in  H2O, 
but  solution  decomp. 

Very  easily  sol.  in  mother  liquor.  (Svens- 
son, Acta  Lund.  1899.  13 .) 

Ammonium  cuprocupric  sulphite,  (NH4)2SO3, 
2Cu2SO3,CuS03+5H2O.  , 

Insol.  in  H2O  and  weak  acids.  Sol.  in 
NH4OH+Aq.  (de  Saint-Gilles,  A.  ch.  (3) 
42.  31.) 

+6^H2O.  Ppt.  (Rosenheim  and  Stein- 
hauser, Z.  anorg.  1900,  25.  98.) 


SULPHITE,  ANTIMONY 


1039 


Ammonium  glucinum  sulphite, 

(NH4)2O,  2G1O,  3SO2+4H2O. 
Ppt.     Very  unstable  in  the  air.     (Rosen- 
heim,  Z.  anorg.  1897,  15.  310.) 

Ammonium  gold  (aurous)  sulphite, 

3(NH4)2SO3,Au2SO3. 

Very  easily  sol.  in  H2O.  Insol.  in  alcohol. 
(Haase,  Z.  Ch.  1869.  535.) 

Ammonium  gold  (aurous)  sulphite  ammonia, 

(NH4)2SO3,  3Au2SO3,  6NH3+H2O. 

Decomp.  by  H2O.  Sol.  in  warm  NH4OH  + 
Aq,  but  decomp.  by  boiling. 

(NH4;Au3(SO3)2,  3NH3+4H2O.  Decomp. 
by  H2O:  (Rosenheim,  Z.  anorg.  1908,  69. 
201.) 

Ammonium  indium  sulphite. 
See  Iridosulphite,  ammonium. 

Ammonium  iron  (ferrous)  sulphite, 

(NH4)2SO3,  FeSO3+zH2O. 
(Berglund.) 

Ammonium  iron  (ferric)  sulphite  sulphate, 

FeSO3SO4NH4+H2O. 

SI.  sol.  in  cold  H2O.  Decomp.  by  cold 
dil.  HC1.  (Hofmann,  Z.  anorg.  1897,  14. 

287.) 

Ammonium  magnesium  sulphite, 

(NH4)2Mg3(SO3)4+18H20. 

Very  si.  sol.  in  H2O.  (Fourcroy  and  Vau- 
quelin.) 

Sol.  in  H2SO3+Aq. 

+5H2O.  Much  more  sol.  in  H2O  than 
MgSO3.  (Rammelsberg.) 

Ammonium  manganous  sulphite,  (NH4)2SO3, 
MnSO3. 

Relatively  easily  decomp.  by  H2O.  (Berg- 
lund, Bull.  Soc.  (2)  21.  213.) 

Not  easily  decomp.  (Gorgeu,  C.  R.  96 
376.) 

Ammonium  mercuric  sulphite,   (NH4)2SO3, 

HgS03. 

Very  easily  sol.  in  H2O,  but  H2O  solution 
gradually  decomp.,  even  in  the  cold. 

Ammonium    nickel    sulphite,    (NH4)2SO3, 

3NiSO3  +  18H2O. 
Sol.  in  H2O.    (Berglund,  B.  7.  469.) 

Ammonium  platinous  sulphite. 
See  Platosulphite,  ammonium. 

Ammonium  potassium  sulphite,  10(NH4)2SO3, 
K2SO3+HH2O. 

Decomp.  by  H2O,  etc.  (Hartog,  C.  R 
109.  221.) 


Ammonium  scandium  sulphate, 

(NH4)2SO3,  Sc2(SO3)3+7H2O. 
Insol.  in  H2O.     Difficulty  sol.  in  H2SO3  + 
Aq.    (Meyer,  Z.  anorg.  1914,  86.  281.) 

Ammonium     silver     sulphite,      (NH4)2SO3, 

Ag2S03. 

Insol.    in    H2O,    but    gradually    decomp. 
hereby.    (Svensson,  B.  4.  714.) 

6(NH4)2SO3,  Ag2SO3  +  19H2O.    Sol.  in  H2O 
without  decomp.     (Svensson.) 

3(NH4)2SO3,  4NH4HSO3,  Ag2SO3  +  18H2O. 
Easily  sol.  in  H2O,  but  decomp.  by  warming. 

Ammonium  sodium  hydrogen  sulphite, 

NH4Na2H(SO3)2+4H2O. 
Not  deliquescent.     (Marignac,  Ann.  Min. 
5)  12.  29.) 

100  pts.  H2O  dissolve  42.3  pts.  salt  at  12.4°, 
and  48.5  pts.  at  15°.    (Schwicker,  B.  22.  1732.) 
+5H2O  =2Na2SO3,         (NH4)2S2O5+H2O. 
^Tauber,  Techn.  J.  B.  1888.  444.) 

Ammonium  tellurium   sulphite,   (NH^SOs, 

TeSO3+zH2O. 
Sol.  in  H2O.    (Berglund,  B.  7.  469.) 

Ammonium  uranyl  sulphite, 

NH4(UO2)(OH)SO3. 

Insol.  in  pure  H2O  More  sol.  in  H2SO3+ 
Aq  than  the  K  salt,  and  less  than  the  Na 
salt.  (Scheller,  A.  144.  240.) 

(NH4)2O,  2UO3,  3SO2. 

(NH4)2O.  4UO3,  5SO2. 

(NH4)2O',  3UO3,  2SO2. 

(NH4)2O,  UO3,  2SO2.  (Kohlschiitter,  A. 
1900,  311.  10.) 

Ammonium  vanadium  sulphite. 
See  Vanadiosulphite,  ammonium. 

Ammonium  vanadyl  sulphite, 
(NH4)2SO3,  VOS03+2H2O. 

Sol.  in  H2O  with  decomp.  (Koppel,  Z. 
anorg.  1903,  36.  184.) 

(NH4)2O,  3VO2,  2SO2+H2O.  Sol.  in  cold 
H2O  without  decomp. 

Easily  sol.  in  mineral  acids  and  alkalies. 

SI.  sol.  in  alcohol  and  ether.  (Koppel 
Z.  anorg.  1903,  36.  182.) 

Ammonium  zinc  sulphite,  (NH4)2SO3,  ZnSOs. 
Sol.  in  H2O.    (Berglund,  B.  7.  469.) 

Ammonium  sulphite  mercuric  chloride, 

2(NH4)2SO3;   HgCl2. 

SI.  sol.  in  cold,  decomp.  by  boiling  H2O. 
(de  St-Giles,  A.  ch.  (3)  36.  95.) 

Antimony  sulphite,  Sb2O3,  3SO2(?). 

Insol.  in  H2O.    (Berzelius.) 

Could  not  be  obtained.  (Rohrig,  J.  pr. 
(2)  37.  241.) 


1040 


SULPHITE,  BARIUM 


Barium  sulphite,  BaSO3. 

Very  si.  sol.  in  H2O.  (Fourcroy  and  Vau 
quelin,  A.  ch.  24.  301.) 

Sol.  in  about  46,000  pts.  H2O  at  16° 
(Autenrieth,  Z.  anal.  1898,  37.  204.) 

Sol.  in  H2SO3+Aq. 

Insol.  in  acetone.  (Naumann.  B.  1904,  37 
4329);  methyl  acetate.  (Naumann,  B.  1909 
42.  3790.) 

Solubility  in  sugar +Aq  at  t°. 


Solvent 

t° 

100  ccm.  of 
solution  con- 
tain g.  BaSOs 

water 
sucrose  +Aq  10°  Brix 
20°      " 

30°      " 
40°      " 
50°      " 
(sat.)"              60°      " 

20 

0.01974 
0.01040 
0.00968 
0.00782 
0.00484 
0.00298 
0.00223 

water 
sucrose  +Aq  10°  Brix 

20°       " 
«                30o      u 

"                40°       " 
50°      " 
(sat.)"               60°      " 

80 

0.00177 
0.00335 
0.00289 
0.00223 
0.00158 
0.00149 
0.00112 

(Rogowicz,  C.  C.  1905,  II.   1223.) 

Barium  cobaltic  sulphite. 

See  Cobaltisulphate,  barium. 

Barium    gold     (aurous)     sulphite,    3BaSO3, 

Au2SO3+:rH2O. 
Ppt.     (Haase.) 

Barium  mercuric  sulphite,  BaSO3,  HgSO3  + 

H20. 
Ppt.     (Earth,  Z.  phys.  Ch.  9.  196.) 

Barium  mercuric  sulphite  chloride, 

BaSO3,  BaCl2,  2HgSO3+3^H2O. 
(Earth,  Z.  phys.  Ch.  1892,  9.  208.) 

Bismuth  sulphite,  basic,  Bi2O3,  3SO2+5H2O. 

Insol.  in  H2O,  alcohol,  or  ether.  SI.  sol.  in 
H2SO3+Aq.  (Rohrig,  J.  pr.  (2)  37.  241.) 

(BiO)2S03,  3(BiOH)S03+H20.  (Seubert 
and  Elten,  Z.  anorg.  1893,  4.  72-5.) 

2(BiO)2SO3,  3(BiOH)SO3+2H2O.  (S.  and 
E.) 

3(BiO)2SO3,  7(BiOH)SO3  +  10H2O.  (S.  and 
E.) 

4(BiO)2SO3,  (BiOH)SO3+5H2O.  (S.  and 
E.) 

9(BiO)2S03,  (BiOH)SO3+2H2O.  (S.  and 
E.) 

Bismuth  cobaltic  sulphite. 
See  Cobaltisulphite,  bismuth. 


Cadmium  sulphite,  CdSO3. 

Difficultly  sol.  in  H2O.  Easily  sol.  in  dil. 
acids.  (Rammelsberg,  Pogg.  67.  256.) 

+2H2O.  Difficultly,  sol.  in  H2O.  Sol.  in 
H2SO3+Aq.  Sol.  rnNH4OH+Aq.  Insol.  in 
alcohol.  (Muspratt,  Phil.  Mag.  (3)  30.  414.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Contains  2>£E2O.  (Deniges,  Bull.  Soc.  (3) 
7.  569.) 

Cadmium  sodium  sulphite,  3CdSO3,  Na2SO8. 
Sol.  in  H2O.    (Berglund,  B.  7.  469.) 

Cadmium  sulphite,  ammonia,  CdSO3,  NH8. 
Decomp.  by  H2O.    Pol.  without  decomp.  in 
hot  NH4OH+Aq.     (Rammelsberg,  Pogg.  67. 
256.) 

Caesium  sulphite,  Cs2SO3. 

Easily  sol.  in  H2O.  SI.  sol.  in  alcohol. 
(Chabrid,  C.  R.  1901,  133.  297.) 

Caesium  hydrogen  sulphite,  CsHSO3. 

Easily  sol.  in  H2O.  SI.  sol.  in  alcohol. 
(Chabrie",  C.  R.  1901,  133.  297.) 

Calcium    sulphite,    basic,    Ca6S6O16  =  6CaO, 

5SO2. 
(Schott,  Dingl.  202.  52.) 

Calcium  sulphite,  CaSO3+2H2O. 

Slowly  effloresces.  Sol.  in  800  pts.  cold 
H2O.  (Berzelius.) 

Insol.  in  H2O.    (Rohrig,  J.  pr.  (2)  37.  230.) 

0.043  g.  is  sol.  in  1  1.  H2O  at  18°.  (Weis- 
berg,  Bull.  Soc.  1896,  (3)  16.  1249.) 

CaSO3  equiv.  to  78  mg.  CaO  is  sol.  in  1  1. 
H2O  at  100°.  (Robart,  C.  A.  1913.  2500.) 

Very  sol.  in  H2SO3+Aq.    See  CaH2(SO3)2. 

InsoL  in  liquid  NH3.  (Franklin,  Am.  Ch.  J. 
898,  20.  827.) 

CaSO3  equiv.  to  37  mg.  CaO  is  sol.  in  1  1. 
2%  cane  sugar +Aq  at  100°.  (Robart,  C.  A. 
1913.  2500.) 

0.0825  g.  is  sol.  in  1 1.  10%  stigar  +Aq.  at 
8°;  0.0800  g.  is  sol.  in  1  1.  30%  sugar  +Aq.  at 
8°.(  Weisberg,  Bull.  Soc.  1896,  (3)  16.  1249.) 

Insol.  in  acetone.     (Krug  and  M'Elroy.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
909,  42.  3790;  ethyl  acetate.  (Naumann, 
B.  1904,  37.  3601.) 

+  KH2O.    (Rammelsberg.) 

Calcium  hydrogen  sulphite,  CaH2(SO3)2. 

Know  only  in  solution. 

100  ccm.  H2O  containing  9  g.  SO2  dissolve 
.553  g.  CaSO3  to  form  a  solution  of  1.06  sp. 
r.  (Gerland,  J.  pr.  (2)  4.  119.) 

Calcium  cobaltic  sulphite. 
See  Cobaltisulphite,  calcium. 


SULPHITE,  CUPROUS  POTASSIUM 


1041 


Cerous  sulphite,  Ce2(SO8)j+3H2O. 

More  sol.  in  cold  than  hot  H2O. 

Solution  gradually  decomposes.  (Berthier, 
A.  ch.  (3)  7.  77.) 

Chromous  sulphite,  CrSO3. 

Precipitate.    Insol.  in  H2O.    (Moberg.) 

Chromium  sulphite,  basic,  Cr2O3,  SO2. 

Colloidal  modification.  Sol.  in  H2O. 

2Cr2O3,  SO2.  Ppt.  (Recoura,  Bull.  Soc. 
1898,  (3)  19.  169.) 

Chromic  sulphite. 

Known  only  in  aqueous  solution,  which  pre- 
cipitates a  basic  salt  on  boiling. 

2Cr2O3,3SO2  +  16H2O.  Precipitate.  (Dan- 
son,  Chem.  Soc.  2.  205.) 

Chromic   potassium   sulphite,   K2O,    Cr2O«, 

2SO2+zH2O. 
Precipitate.    (Berglund,  B.  7.  470.) 

Cobaltous  sulphite,  basic. 

Ppt.       Decomp.     by     H2O.       (Berthier.) 
Co(OH)2,     5CoSO3  +  10H2O.     Ppt.     (Seu- 

bert  and  Elten,  Z.  anorg.  1893,  4.  89.) 

Co(OH)2,  10CoSO3  +  15H2O.    (Seubert  and 

Elten.) 

Cobaltous  sulphite,  CoSO3. 

+3H2O.  Nearly  insol.  in  H2O.  Sol.  in 
H2SO  8  +  Aq.  (Rammelsberg. ) 

Partly  sol.  in  NH4OH+Aq. 

+5H2O.  Insol.  in  H2O.  Sol.  in  H2SO3  + 
Aq.  (Muspratt,  A.  30.  282.) 

Cobaltocobaltic  sulphite. 
See  Cobaltisulphite,  cobaltous. 

Cobaltic  sulphite  with  3M2SO8. 
See  Cobaltisulphite,  M. 

Cobaltous  potassium  sulphite,  CoSO8,  K2SO3 

+zH20. 

Insol.  in  H2O;  easily  sol.  in  HCl+Aq. 
(Schultze,  J.  B.  1864.  270.) 

Cobaltic    potassium    sulphite,    Co2(SO8)s, 

K2SO8. 

SI.  sol.  in  H2O;  easily  sol.  in  H2SO3+Aq  or 
HCl+Aq.  (Schultze.) 

Cobaltous    sodium    sulphite,    3CoO,    Na2O, 

3S02. 

Insol.  in  H2O.  Easily  sol.  in  HCl+Aq. 
(Schultze.) 

Cobaltic    sodium    sulphite,    Co208,    Na2O 

3S02. 
SI.  sol.  in  H2O.    (Schultze.) 


Cuprous  sulphite,  Cu2SO8+H20. 

(a)  Red.  SI.  sol.  in  H2O.  Sol.  in  NH4OH 
or  HCl+Aq.  (Rogojski,  J.  B.  1861.  366.) 

Could  not  be  obtained  by  St.  Gilles  or 
Svensson  (B.  4.  713). 

Insol.  in  H2O,  alcohol,  or  ether.  (Etard,  C. 
R.  95.  38.) 

Composition  is  (Cu2)8Hi6(SO4)8,  "Cuprous 
isosulphite,"  according  to  fitard. 

+  }^H2O.  Etard's  formula,  Cu2SO8+H2O 
s  incorrect. 

The  salt 'is  almost  colorless.  (Ramberg 
I.  phys.  Ch.  1909,  69.  512.) 

(j8)  White.  Normal  salt.  Insol.  in  H2O, 
alcohol,  or  ether.  (Etard.) 

Cupric  sulphite,  basic,  4CuO,  SO2+7H2O. 

Insol.  in  H2O,  and  decomp.  by  washing 
therewith.  (Millon  and  Commaille.) 

7CuO,  4SO2+8H2O.  Sol.  in  dil.  H2SO4. 
(Seubert  and  Elten,  Z.  anorg.  1893,  4.  48.) 

3CuO,  2SO2  +  1^H2O.  SI  sol.  in  H2O. 
(Newbury,  Am.  Ch.  J.  14.  232.) 

7CuO,  4SO2+8H2O,  or  4CuSOa,  3Cu(OH)2 
+5H2O.  Sol.  in  dil.  H2SO4+Aq.  (Seubert 
and  Elten,  Z.  anorg.  1893,  4.  50.) 

Cuprocupric  sulphite,  CuSO8,  Cu2SO8+2H2O. 

Nearly  insol.  in  cold  H2O.  Decomp.  by 
boiling. 

Sol.  in  H2SO3+Aq,  HC1,  or  NH4OH+Aq. 
(Berthier.) 

Sol.  in  very  dil.  HNO3+Aq.  (Dopping, 
J.  B.  1861.  365.) 

Insol.  in  H2SO3,  HC2H3O2,  or  Cu  salts +Aq. 
(de  St.  Gilles.) 

+5H2O.  Insol.  in  H2O.  Easily  sol.  in 
H2SO3+Aq,  HC2H3O2+Aq,  in  cupric  salts 
+Aq,  NH4OH+Aq,  or  HCl+Aq.  (de  St. 
Gilles,  A.  ch.  (3)  42.  34.) 

Composition  is  ((^CugHiiiiSO^B^aiHiO, 
acid  cuproso cupric  octosulphite."  (Etard, 
C.  R.  96.  1475.) 

Cuprous  ferroferric  sodium  sulphite,  Cu2O, 

2FeO,  Fe2O3,  Na2O,  6SO2+16H2O. 

Sol.  in  about  1000  pts.  H2O. 

Sol.  in  cold  dil.  H2SO4+Aq;  sol.  in  cold 
dil.  HCl+Aq  with  a  residue  of  Cu2Cl2. 
(Stromeyer,  A.  109.  237.) 

Cuprous  lithium  sulphite,  Cu2SO8,  Li2SO3+ 

2H20. 

Insol.  in  H2O,  but  gradually  decomp. 
thereby.  (Etard,  C.  R.  96.  138.) 

Cupric   mercuric   sulphite,    CuSOj,    HgSO8. 
Sol.  in  H2O  in  all  proportions,  but  decomp. 
on  boiling. 

Cuprous  potassium  sulphite,  Cu2SOt, 

K2S08  (?). 

(Vohl,  J.  pr.  95.  219.) 
+2H2O.      Sol.    in    H2O    with    decomp. 


1042 


SULPHITE,  CUPROCUPRIC  POTASSIUM 


(Rosenheim  and  Steinhauser,  Z.  anorg.  1890, 
25.  96.) 

Cu2SO3,  2K2SO3.  (Chevreul,  Graham, 
etc.) 

Does  not  exist.    (Svensson.) 

Cu2O,  3K2O,  6SO2+7H2O=4KHSO3, 
K2SO3,  Cu2SO3+5H2O.  Decomp.  by  H2O. 
(Svensson,  B.  4.  713.) 

Could  not  be  obtained.  (Rosenheim  and 
Steinhauser.) 

Cu2O,  4K2O,  8S02+3H2O=6KHSO3, 
K2SO3,  Cu2SO3.  Decomp.  by  HzO.  (Svens- 
son.) 

Could  not  be  obtained.  (Rosenheim  and 
Steinhauser.) 

Cu2SO3,  8K2SO3  +  16H2O.  Sol.  in  H2O 
with  decomp.  (Rammelsberg,  Pogg.  57.  391.) 

Does  not  exist,  according  to  Svensson. 

Cuprocupric  potassium  sulphite,  3Cu2S03, 
3CuSO3,  K2SO3. 

Properties  as  cuprous  potassium  sulphite. 
(Rogojski,  J.  B.  1851.  367.) 

2Cu2SO3,  CuSO3,  K2SO3+5H2O.  Insol. 
in  H2O  and  weak  acids,  (de  St-Gilles.) 

Cu2SO3,  4CuSO3,  JK2SO8+16H20.  De- 
comp. by  H2O.  (Rosenheim  and  Steinhauser. 

Cuprous  sodium  sulphite,  Cu2SO3,  Na2SO3. 
+2H2O.     Decomp.  by  H2O.     (Svensson, 
1870.) 

+  11H2O.  Insol.  in  cold  H2O,  but  decomp. 
by  excess.  (Etard,  C.  R.  95.  138.) 

2Cu2SO3,  3Na2SO3+29H2O.  Insol.  in  H2O. 
(Rosenheim  and  Steinhauser,  Z.  anorg.  1900. 
25.  94.) 

Cu2SO3,  5Na2SO3+38H2O.  Decomp.  by 
H2O.  (Svensson.) 

Cu2SO3,  7Na2SO3-|-19H2O.  Completely 
sol.  in  H2O,  but  solutions  decomp.  on  stand- 
ing. (Svensson.) 

' '  Cuprous  sodium  oc/osulphite, ' ' 
(Cu2)3Hi0Na16S8O32+43H2O.    (Etard.) 

5Cu2SO3,  2Na2SO3+30H2O.  Easily  de- 
comp. (Rosenheim  and  Steinhauser,  Z. 
anorg.  1900,  25.  94.) 

Cuprocupric  sodium  sulphite. 

Cu2SO3,  2CuSO3,  2Na2SO3+6H2O. 

Nearly  insol.  in  cold,  decomp.  by  hot  H2O. 
(Rosenheim  and  Steinhauser.  Z.  anorg.  1900. 
25.  95.) 

+8H2O.  Decomp.  by  H2O.  (Rosenheim 
and  Steinhauser.) 

Cuprocupric  sodium  hydrogen  sulphite. 

Na8Cu?0I(CuDH2(S04)8,6H4(S04)  +  5H2O. 
Insol.  in  H2O.    (Etard,  C.  R.  94.  1422.) 
(Cu!)Cu»Na8H18(S04)8.    (Etard.) 

Copper  sodium  sulphites. 

Doubtless  many  of  the  compds.  described 
in  this  class  are  in  reality  isomorphic  mixtures 
whose  composition  depends  upon  the  temp, 
and  cone,  of  the  solution  in  which  pptd. 


(Rosenheim  and  Steinhauser,  Z.  anorg.  1900, 
25.  92-95.) 

Didymium    sulphite,    Di2(SO3)3+3H2O,     or 

6H2O. 

Precipitate.  Insol.  in  H2O.  Sol.  in  H2SO3 
+Aq,  from  which  it  is  reprecipitated  by 
heating,  redissolving  on  cooling^  (Marignac, 
A.  ch.  (3)  38.  167.) 

Erbium  sulphite,  Er2(SO3)3-|-3H2O. 
Precipitate. 

Glucinum  sulphite,  basic,  2G1SO3,  9G1(OH)2 

+6H2O. 

Ppt.     (Seubert,  Z.  anorg.  1893,  4.  52.) 
G1SO3,  G1O.    Decomp.  by  H2O  or  alcohol. 

(K.  and  M.) 
3G1SO3,  G1C.    Sol.  in  alcohol.    (K.  and  M.) 

Glucinum  sulphite,  G1SO3. 

Decomp.  by  H2O  or  alcohol.  (Kruss  and 
Moraht,  B.  23.  734.) 

Glucinum  potassium  sulphite, 

2G1SO3,  K2SO3+9H2O. 
Unstable  in  the  air.    (Rosenheim,  Z.  anorg. 
1897,  15.  310.) 

Gold  (aurous)  potassium   sulphite,  Au2S03, 

3K2SO3. 
Very  sol.  in  H2O;  insol.  in  alcohol.    (Haase.) 

Gold   (auric)   potassium  sulphite,  Au2O3, 
5K2O,  8SO2+5H2O=5K2SO3,  Au2(SO3)8 
+5H2O. 

Sol.  in  H2O  with  decomp. 
Decomp.    by    acids;    insol.    in    alkalies. 
(Fremy,  A.  79.*  46.) 

Gold  (auric)  potassium  sulphite, 

Au2(SO3)3,  5K2SO3+10H2O. 
(Rosenheim  and  Hertzmann,  Z.  anorg.  1908. 
59.  199.) 

Gold  (auric)  potassium  sulphite  ammonia, 

Au2(SO3)3,  3K2SO3,  4NH3+4H2O. 
As  the  corresponding  NH4  salt.     (Rosen- 
heim   and  Hertzmann,  Z.  anorg.    1908,  59. 

202.) 

Gold    (aurous)    sodium    sulphite,    Au2SO3, 

3Na2SO3+3H2O. 
Sol.  in  less  than  1  pt.  H2O.    Insol.  in  alcohol 

(Hasse.) 

+5H2O.    (Himly.) 

Gold  (auric)  sodium  sulphite, 

Au2(SO3)^,  5Na2SO3+28H2O. 
As  K  salt.      (Rosenheim  and  Hertzmann, 
anorg.  1908,  59.  199.) 


SULPHITE,  MANGANOUS 


1043 


Gold  (aurous)  sulphite  ammonia,  3Au2O, 
4S02,  8NH3+4H20. 

SI.  sol.  in  H2O  with  decomp.  Decomp.  by 
acids. 

SI.  sol.  in  cold,  more  easily  in  hot  NH4OH  + 
Aq.  Decomp.  by  boiling.  (Hasse.  Zeit.  Ch. 
1869.  535.) 

Gold  (auric)  sulphite  ammonia, 

Au3(S03)2,  4NH3+4H20. 
Ppt.    Decomp.  in  moist  air  and  in  neutral 
solution     (Herzmann,    Z.   anorg.    1908.   59. 
198.) 

Indium  sulphite,  2In2O3,  3S02+8H2O. 
Insol.  in  H2O.    (Bayer,  A.  168.  372.) 

Iridium  sulphite,  Ir2(SO3)3+6H2O. 

Scarcely  sol.  in  H2O;  easily  sol.  HCl+Aq. 
(Birnbaum,  A.  136.  179.) 

Iridyl  sulphite,  (IrO)SO3+4H20. 

Insol.  in  H2O.  Sol.  in  HC1  or  H2SO4+Aq. 
(Birnbaum.) 

Iridous    potassium     sulphite,     IrO,     .3K2O, 

5SO,(f). 

SI.  sol.  in  H2O,  more  sol.  in  KOH+Aq. 
Easily  sol.  in  HCl+Aq.  (Glaus,  J.  pr.  42. 
359.) 

Iridous  sulphite  potassium  chloride. 
See  Iridosulphite,  potassium. 

Iridium  sulphite  with  M2SO3. 
See  Iridosulphite,  M. 

Iron  (ferrous)  sulphite,  FeSO3+2^H2O. 

Very  si.  sol.  in  H2O.  Easily  sol.  in  H2SO3+ 
Aq.  Insol.  in  alcohol,  but  sol.  therein  in 
presence  of  SO2.  (Muspratt.) 

Iron  (ferric)  sulphite,  Fe2O3,  S02+6H2O. 
Very  si.  sol.  in  H2Q.    Sol.  in  acids.   (Koene.) 
2Fe2O3,  3SO2.     Deliquescent;  decomp.  by 

H2O  into  SO2  and  above  comp. 
3Fe2O3,  SO2+7H2O.    Ppt. 

Iron  (ferroferric)  potassium  sulphite,  FeSO3, 

(FeO)2SO3,  2K2SO3. 
Ppt.    (Berglund.) 

Iron  (ferric)  potassium  sulphite,  K2O,  Fe2O3, 
3SOS+2H20. 

Sol.  in  H2SO3+Aq.  (Koene,  Pogg.  63. 
453.) 

Fe2O3,  2K2Q,  3SO2+5H2O.  Ppt.  (Mus- 
pratt, Phil.  Mag.  (3)  30.  414.) 

Iron  (ferric)  potassium  sulphite  sulphate, 
FeS03S04K. 

SI.  sol.  in  cold  H2O. 

Sol.  in  20%  HC1;  decomp.  on  boiling. 
(Hofmann,  Z.  anorg.  1897,  14.  286.) 


Fe(SO3)2SO4K3.  Almost  insol.  in  cold 
H2O.  Decomp.  by  boiling  with  dil.  acids. 
(Hofmann.) 

Fe2(SO3)4SO4K4+5H2O.  Insol.  in  cold 
H2O;  sol.  in  cold  20%  HCl+Aq;  decomp.  on 
boiling  with  H2O.  (Hofmann.) 

Iron  (ferric)  sodium  sulphite  sulphate, 

Fe(SO3)2SO4Na3+6H2O. 
Almost  insol.  in  H2O. 

Decomp.  by  boiling  with  dil.  acids.  (Hof- 
mann, Z.  anorg.  1897,  14.  289.) 

Iron  (ferric)  sodium  hydrogen  sulphite  sul- 
phate, FeSO4(SO3)4H2Na2+2H2O. 
Only  very  si.  sol.  in  H2O.      (Hofmann.) 

Lanthanum  sulphite,  La2(SO3)3+4H2O. 
Precipitate.    (Cleve.) 

Lead  sulphite,  PbSO8. 

Insol.  in  H2O.  Decomp.  by  acids.  SI.  sol. 
in  H2SO3+Aq.  (Rohrig,  J.  pr.  (2)  37.  233.) 

Lithium  sulphite,  Li2SO3+6H2O. 

Sol.  in  H2O;  precipitated  from  aqueous 
solution  by  abs.  alcohol.  (Danson,  Chem. 
Soc.  2.  205.)  Sol.  in  H2SO3+Aq. 

+H2O.  SI.  sol.  in  alcohol,  and  still  less 
sol.  in  ether.  (Rohrig,  J.  pr.  (2)  37.  225.) 

+2H2O.    (Rohrig.) 

Lithium  potassium  sulphite,  LiKSO»+^H2O. 
Easily  sol.  in  H2O.     (Rohrig,  J.  pr.  (2)  37. 
251.) 

Lithium  sodium  sulphite,  6Li2SO3,  Na2S08+ 

8H2O. 
Sol.  in  H2O.    (Rohrig.) 

Magnesium   sulphite,   MgSO3+6H20. 

Sol.  in  20  pts.  cold,  and  in  less  hot  H2O.  (Fourcroy 
and  Vauquelin.) 

Sol.  in  80  pts.  cold,  and  in  120  pts.  boiling 
H2O.  (Hager,  C.  C.  1875.  135.) 

More  easily  sol.  in  H2SO3+Aq. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  828.) 

Precipitated  from  aqueous  solution  by 
alcohol. 

+3H2O.    (Rohrig,  J.  pr.  (2)  37.  234.) 

Manganous  sulphite,  MnSO3+2H20. 

Insol.  in  H2O,  alcohol,  or  ether.  Easily  sol. 
in  acids,  also  in  H2SO3+Aq. 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

+2HH2O.  (Rammelsberg.) 
.  +3H2O.  Sol.  in  10,000  pts.  cold,  and  5000 
pts.  hot  H2O;  more  sol.  in  cone.  Mn  salts+Aq; 
sol.  in  1000  pts.  H2CO3+Aq.  100  pts.  H2SO3 
+Aq  dissolve  15-17  pts.  (Gorgeu,  C.  R.  96. 
341.) 


1044 


SULPHITE,  MANGANOUS  POTASSIUM 


Salt  with  2^H2O  is  the  only  one -which 
exists.  (Rohrig,  J.  pr.  (2)  37.  2.) 

Manganous  potassium  sulphite,  2MnSO3, 
K2SO». 

Insol.  in  H2O,  even  when  boiling.  (Gorgeu, 
C.  R.  96.  376.) 

MnSO3,  K2SO3.    Sol.  in  H2O.    (Gorgeu.) 

Manganous  sodium  sulphite,  MnSO3,  Na2SO3 
+H20. 

Insol.  in  hot  H2O,  but  decomp.  by  cold  H20. 
(Gorgeu.) 

4MnSO3,  Na2SO3.  Insol.  in  H2O.  (Gor- 
geu.) 

Mercuric  sulphite,  2HgO,  SO2. 

Insol.  in  H2O.  Sol.  in  HC1,  alkali  sul- 
phites with  subsequent  decomp.,  and  in  KCN 
+Aq.  (de  St-Gilles,  A.  ch.  (3)  36.  80.) 

HgSO3.  Decomp.  by  cold  H2O.  (de  St- 
Gilles.) 

Does  not  exist.  (Divers  and  Shimidzu, 
Chem.  Soc.  49.  553.) 

HgO,  2SO2+H2O.  Sol.  in  H20,  but  de- 
comp. by  boiling,  (de  St-Gilles.)  Exists  only 
in  aqueous  solution.  (Divers  and  Shimidzu.) 

Mercuromercuric  sulphite,  Hg3(SO3)2+ 
2H2O  =  Hg2SO3,  HgS03. 

Very  efflorescent.  Insol.  in  H2O.  Decomp. 
by  hot  H2O.  Insol.  in  dil.  HNO3  or  H2SO4  + 
Aq. 

+4H2O.    Very  efflorescent. 

Ifypomercurosic  sulphite,  Hg4(S03)2+H2O. 
Insol.  in  H2O,  but  easily  decomp.  on  stand- 
ing therewith.  Almost  absolutely  insol.  in 
dil.  HNO3  or  H2S04+Aq.  (Divers  and 
Shimidzu.) 

Mercuric    orn/sulphite,   Hg(SO2OHgO)2Hg+ 

H2O. 

Insol.  in  H2O.  Decomp.  by  hot  H2O.  In- 
sol. in  dil.  HNO3  or  H2SO4+Aq.  Sol.  in 
H2SO3-|-Aq.  (Divers  and  Shimidzu.) 

Mercuric  potassium  sulphite,  basic, 

K2O,  2HgO,  2SO2. 
(Earth.  Z.  phys.  Ch.  1892,  9.  210.) 
K2O,  3HgO,  3SO2.    Insol.  in  H2O.    Partly 

sol.  in  KOH+Aq.    (Barth.) 

Mercuric  potassium  sulphite,  HgSO3,  K2SO3 

+H20. 

SI.  sol.  in  cold  H2O.  Decomp.  on  boiling, 
(de  St-Gilles,  A.  ch.  (3)  36.  90.) 

Mercuric      potassium      sulphite      mercuric 

chloride,  K2Hg(S03)2,  HgCl2. 
Decomp.  by  H2O.     (Barth,  Z.  phys.  Ch. 
1892,  9.  206.) 


Mercuric  silver  sulphite,  HgSO3,  Ag2SO3  + 

2H2O. 

Decomp.  rapidly;  insol.  in  H2O.  (Barth,, 
Z.  phys.  Ch.  9.  195.) 

Mercuric  sodium  sulphite,  HgS03,  Na2SO8  + 
H2O. 

Sol.  in  H2O.    (de  St-Gilles.) 

Sol.  in  25  pts.  cold  H2O,  and  decomp.  on 
heating.  (Divers  and  Shimidzu.) 

+2H2O  =  Na2(SO3)2Hg+2H2O.      (Barth, 
Z.  phys.  Ch.  9.  193.) 

2HgSO3,  Na2SO3+H2O.  Much  more  sol. 
in  H2O  than  the  above  comp.  especially  on 
heating,  (de  St-Gilles.) 

Does  not  exist.    (Divers  and  Shimidzu.) 

Mercuric  strontium  sulphite,  HgS03,  SrSO8  + 

2H2O. 
Ppt.    (Barth.) 

Mercuric  sulphite  ammonium  bromide, 

HgSO3,  NH4Br. 

As  NH4C1  comp.  (Barth,  Z.  phys.  Ch. 
1892,  9.  215.) 

Mercuric  sulphite  ammonium  chloride, 
HgS03,   NH4C1. 

As  K  salt.    (Barth.) 

Mercuric  sulphite  potassium  chloride, 

HgSO3,  KC1. 
Sol.  in  H2O.    (Barth.) 

Mercuric   sulphite  sodium  chloride,  HgSO», 

NaCl+H20. 
Sol.  in  H2O.    (Barth.) 

Nickel  sulphite,  basic,  2NiSO3,  Ni(OH)2+ 

6H2O. 

Ppt.  (Seubert  and  Elten,  Z.  anorg.  1893, 
4.91.) 

Nickel  sulphite,  NiSO3+4H20. 

Insol.  in  H2O.  Sol.  in  HCl+Aq.  with 
evolution  of  SO2.  (Muspratt,  A.  60.  259.) 

+6H2O.  Insol.  in  H2O.  Sol.  in  H2SO3  + 
Aq.  (Rammelsberg,  Pogg.  67.  391.) 

Nickel  sulphite  ammonia,   NiSO3,   3NH8  + 

3H20. 

Sol.  in  little  H2O.  Decomp.  by  much  H20 
or  heat.  (Rammelsberg,  Pogg.  67.  245.) 

Osmious  sulphite,  OsSO8. 

Insol.  in  H2O.  Easily  sol.  in  HCl+Aq 
without  evolution  of  SO2.  Very  slowly  de- 
comp. by  KOH+Aq.  (Claus.) 

Osmious  potassium  sulphite,  OsS08,  2K2SO«, 

2KHSO3+4H2O. 
Nearly  insol.  in  H2O. 


SULPHITE,  SCANDIUM 


1045 


Osmious  potassium  sulphite  chloride,  OsO, 

2S02,  6KC1. 
Easily  sol.  in  H2O. 

PaUadous  sodium  sulphite,  PdSO3,  3Na2S03 
Na6Pd(SO3)4+2H2O. 


Sol.  in  hot  H2O.  Sol.  in  NaOH+Aq  or 
H2SO3+Aq.  (Wohler  and  Frerichs,  A.  174. 
199.) 

Platinous  sulphite,  PtO2,  2SO2. 

Easily  sol.  in  H2O  or  alcohol.  (Dobereiner, 
J.  pr.  16.  315.) 

Formula  is  PtSO3.     (Gmelin.) 

PtSO3,  H2SO3.     (Birnbaum,  A.  139.  172.) 

Platinic    potassium    sulphite,    PtO2,    S02, 

K2S03+H20. 

Sol.  in  KOH+Aq.  (Birnbaum,  A.  139. 
173.) 

Platinic  sodium  sulphite,  PtO2,  SO2,  2Na2SO3 

+2H20. 
Sol.  in  H2O.    (Birnbaum.) 

Platinous  sulphite  with  M2SO3. 
See  Platosulphite,  M. 

Platinum  sulphite  ammonium  chloride. 
See  Chloroplatosulphite,  ammonium. 

Potassium  sulphite,  K2SO3-f2H2O. 

Somewhat  deliquescent.  Sol.  in  1  pt.  cold, 
and  still  less  hot  H2O.  (Fourcroy  and  Vau- 
quelin,  A.  ch.  24.  254.) 

Insol.  in  liquid  NH3.  (Franklin.  Am.  Ch. 
J.  1898,  20.  829.) 

Very  slightly  soluble  in  alcohol.  Insol.  in 
ethyl  acetate.  (Casaseca,  C.  R.  30.  821.) 

Potassium  hydrogen  sulphite,  KHSO3. 
Sol.  in  H2O.    Insol.  in  absolute  alcohol. 

Potassium  p^/rosulphite,  K2S2O6. 

Slowly  sol.  in  H2O.  Very  si.  sol.  in  alcohol; 
insol.  in  ether.  (Muspratt,  A.  50.  259.) 

Potassium   rhodium    sulphite,    3K2SO8, 

Rh2(SO3)3+6H2O. 
See  Rhodosulphite,  potassium. 

Potassium  ruthenium  sulphite, 

O[Ru(S03)4K6J2+2H2O. 
Ppt.    (Miolati,  C.  C.  1901,  1.  501.) 

Potassium  sodium  sulphite,  KNaSO8. 
Sol.  in  H2O.    (Spring,  B.  7.  1161.) 
+  1,  and  2H2O.     (Schwicker,  B.  22.  1731.) 
Isomeric    salts,    KSO3Na    and    NaSO3K. 

(Earth,  Z.  phys.  Ch.  9.  176.) 


Potassium  sodium  hydrogen  sulphite, 

KNa2H(SO3)2+4H20. 
Easily  sol.  in  H2O;  100  pts.  H2O  dissolve 
69  pts.  salt  at  15°.    (Schwicker,  B.  22.  1731.) 
K2NaH(SO3)2+3H2O.    (Schwicker.) 

Potassium  uranyl  sulphite,  K(UO2)(OH)SO8. 
Insol.    in   H2O,    but   sol.    in    H2SO3+Aq. 

(Scheller.) 

K2O,  2UOS,  3SO2.    (Kohlschiitter,  A.  1900, 
311.  10  et  sea.) 

K2O,  4UO3,  5SO2.    (K.) 

K2O,  3UO3,  2SO2.    (K.) 

K2O,  U03,  2SO2.    (K.) 

Potassium  vanadium  sulphite. 
See  Vanadiosulphite,  potassium. 

Potassium  vanadyl  sulphite,  K2SO3, 


Sol.  in  H2O  without  decomp.  and  can  be 
recryst.  therefrom.  (Koppel  and  Behrendt, 
B.  1901,  34.  3932.) 

K2O,  3VO2,  2SO2.  Sol.  without  decomp. 
m  cold  and  hot  H2O.' 

Insol.  in  alcohol  and  ether.  (Koppel,  Z. 
anorg.  1903,  36.  182.) 

Potassium  zinc  sulphite,  K2SO3,   3ZnS03  + 


Sol.  in  H2O  with  decomp.  (Berglund,  Acta 
Lund.  1872.) 

Rhodium  sulphite,  Rh2(SO3)3+6H2O. 
Sol.  in  H2O.    Insol.  in  alcohol.    (Claus.) 

Rhodium  sodium  sulphite. 
See  Rhodosulphite,  sodium. 

Ruthenium  sulphite,  Ru2(S03)8. 

Colloidal  substance,  sol.  in  a  large  quantity 
of  H2O.  (Lucchesi,  Gazz.  ch.  it.  1900,  30. 
(2)  71.) 

Ruthenium  sodium  sulphite,  Na7Ru(SO3)5 

+2H20. 
Ppt.    (Miolati,  C.  C.  1901,  I.  501. 

Samarium  sulphite,  Sm2(SO3)3. 
Amorphous  precipitate.    (Cleve.) 

Scandium  sulphite,  Sc2(SO8)3. 

Insol.  in  cold  H2O.     SI.  sol.  in  hot  H2O. 

Sol.  in  excess  of  sodium  sulphite  when 
heated.  (Crookes,  Phil.  Trans.  1910,  210.  A. 
363.) 

+6H2O.    Very  si.  sol.  in  H2O. 

Decomp.  by  boiling  with  H2O'  with  separa- 
tion of  H2SO3.  (R.  J.  Meyer.  Z.  anorg.  1914, 
86.281.) 


1046 


SULPHITE,  SELENIUM 


Selenium  sulphite,  SeS03. 

Correct  composition  for  "selenium  sulph- 
oxide."  (Divers,  Chem.  Soc.  49.  583.) 

Silver  sulphite,  Ag2SO«. 

Very  si.  sol.  in  cold  H2O.  Decomp.  on 
heating. 

Solubility  in  H2O  is  <  1:20,000.  (Bau- 
bigny,  C.  R.  1909,  149.  858.) 

Easily  sol.  in  NH4OH+Aq,  and  alkali 
sulphites+Aq.  Insol.  in  H2SO3+Aq.  .De- 
comp. by  strong  acids,  but  not  by  acetic  acid. 
(Berthier,  A.  ch.  (3)  7.  82.)  _ 

Easily  sol.  in  alkali  thiosulphates+Aq. 
(Herschel.) 

Cold  NaHSOs+Aq  dissolves  a  considerable 
amount  of  Ag2SO3.  ('Rosenheim  and  Stein- 
hauser,  Z.  anorg.  1900,  25.  78.) 

Practically  insol.  in  HNO3+Aq  or  dil. 
AgNOs+Aq,  also  in  H2SO3+Aq.  (Divers, 
Chem.  Soc.  49.  579.) 

Silver  sodium  sulphite,  Ag2SO3,  Na2SO8-f- 

H20. 
Decomp.  by  H2O.     (Svensson,  B.  4.  714.) 

Sodium  sulphite,  Na2SO8. 

100  pts.  dissolve  at  0°,  14.1  pts.;  at  20°,  25.8 
pts.  ;  at  40°,  49.5°  pts.  Na2SO3.  (Kremers, 
Pogg.,99.  50.)  Maximum  solubility  is  at  33.° 
(Mitscherlich.) 

Solubility  in  100  pts.  H2O  at  t°. 


t° 

Pts.  NazSOs 

37.2 

44.08 

33.5 

39.64 

29.0 

34.99 

23.5 

29.92 

18.2 

25.31 

10.6 

20.01 

5.9 

17.61 

2.0 

14.82 

—1.9 

13.09 

t° 

Pts.  Na2SO3 

60.4 
59.8 
59.8 
59.8 

28.29 
28.29 
28.65 
28.75 

37.0 
37.0 
47.0 
47.0 
55.6' 
84.0 

28.01 
28.07 
28.19 
28.07 
28/21 
28.26 

The  temp,  at  which  Na2SO3+7H2O  changes 
into  Na2SO3  is  about  21.6°. 
(Hartley  and  Barrett,  Chem.  Soc.  1909,  95. 
1183.) 

See  also  +7H2O. 

Sp.  gr.  of  sat.  solution  at  15°  =  1.21. 
(Greenish  and  Smith,  Pharm.  J.  1901,  66. 
774.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Insol.  in  alcohol. 

Insol.  in  ethyl  acetate.  (Casaseca,  C.  R. 
30.  821.);  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Insol.  in  benzonitrile.  (Naumann,  B. 
1914,  47.  1370.) 


-f-7H2O.    Decomp.  slowly  on  air. 

Sol.  in  4  pts.  H2O  at  15°  with  absorption 
of  heat  (Dumas),  and  in  1  pt.  boiling  H2O 
(Fourcroy) . 

Solubility  in  100  pts.  H2O  at  t°. 


Supersolubility    curves    have    also    been 
plotted  for  ice  and  Na2SO3+7H2O. 
(Hartley  a'nd  Barrett,  Chem.  Soc.  1909,  95. 
1181.) 

+10H2O.  Efflorescent.  Somewhat  less 
sol.  than  above  salt.  (Muspratt.) 

Sodium  hydrogen  sulphite,  NaHSO3. 
:    More  difficulty  sol.  in  H20  than  NaHCO3, 
and  is  precipitated  by  alcohol  from  aqueous 
solution.     (Muspratt.) 

Insol.  in  acetone.  (Eidmann,  C.  C.  1899, 
II.  1014;  Naumann,  B.  1904,  37.  4329) 
methyl  acetate.  (Naumann,  B.  1909,  42. 
3790.) 

+4H2O.    (Clark.) 

Sodium  pyrosulphite,  Na2S206. 
Decomp.  gradually  on  the  air. 

Sodium  uranyl  sulphite,  Na(U02)(OH)SO3. 

SI.  sol.  in  H2O.  More  sol.  in  H2S03+Aq 
than  the  K  salt.  (Scheller.) 

Na2O,  2UO3,  3SO2. 

:    Na2O,    3UO3,    2SO2.      (Kohlschutter;    A. 
1900,  311.  10  et  seq.) 

Sodium  vanadyl  sulphite,  Na2O,  2SO2, 
V02+5H20. 

Sol.  in  H2O  with  decomp. 

Na2O,  2SO2,  3VO2+4H2O.  Sol.  in  cold 
H2O;  decomp.  on  heating.  (Koppel,  B.  1901, 
34.  3933.) 

Sodium    zinc    sulphite,    Na2S03,    3ZnS03-f 


Sol.  in  H2O  with  decomp.    (Berglund.  Acta 
Lund,  1872.) 

Sodium   sulphite   silver  chloride,  3Na2S08, 

AgCl+21H2(X 
Sol.  in  H2O.    (Svensson.) 


SULPHURYL  TITANIUM  CHLORIDE 


1047 


Strontium  sulphite,  SrSO3. 

Precipitate.  Almost  insol.  in  H2O.  Sol.  in 
H2SO3+Aq.  (Muspratt.) 

Sol.  in  about  30,000  pts.  H2O  at  16-18°. 
(Autenrieth,  Z.  anal.  1898,  37.  293.) 

Abundantly  sol.  in  H2SO3+Aq.     (Rohrig.) 

Tellurium  sulphite,  TeSO». 

Correct  composition  of  "tellurium  sulph- 
oxide."  (Divers,  Chem.  Soc.  49.  583.) 

Thallous  sulphite,  T12SO3. 

SI.  sol.  in  cold,  easily  in  hot  HjSOs+Aq. 
(Rohrig,  J.  pr.  (2)  37.  229.) 

100  pts.  H2O  dissolve  3.34  pts.  at  15.5°. 
Easily  sol.  in  hot  H2O;  insol.  in  alcohol. 
(Seubert  and  Elten,  Z.  anorg.  2.  434.) 

Thallous    vanadyl     sulphite,    2T12SO8, 

V203S03+4H20. 
(Gain,  A.  ch.  1908,  (8)  14.  278.) 
T12SO3,  3V2O3SO3+8H2O.    (Gain.) 

Thorium  sulphite,  Th(SO3)2+H2O. 

Precipitate.    (Cleve.) 

Tin  (stannous)  sulphite,  5SnO,  2SO2-fzH2O. 

Ppt.  Partly  sol.  in  H2SO3+Aq.  (Rohrig, 
J.  pr.  (2)  37.  249.) 

+20HoO.     (Rohrig.) 

8SnO,  2SO2+20H2O. 

HSnO,  2SO2+20H2O.    (Rohrig.) 

Uranous  sulphite,  basic,  U(OH)2SO8+H20. 

Insol.  in  H2O.  Easily  sol.  in  acids.  Sol. 
in  H2SO3+Aq,  but  is, soon  decomp.  (Ram- 
melsberg.) 

Uranyl  sulphite,  basic,  3UO2(OH)2, 

5(UO2)SO3+10H20. 
(Seubert  and  Elten,  Z.  anorg.  1893,  4.  80.) 

Uranyl  sulphite,  (UO2)SO8+4H2O. 

Insol.  in  H2O.  Sol.  in  H2SO3+Aq  or  alco- 
holic solution  of  SO2.  (Rohrig,  J.  pr.  (2)  37. 
240.) 

Vanadyl  sulphite,  3VO2,  2SO2+4^H2O. 

Decomp.  slowly  on  standing. 

Sol.  in  H2O  without  apparent  decomp. 
(Koppel,  Z.  anorg.  1903,  35.  186.) 

2V2O4,  3SO2-MOH2O.  Sol.  in  H2O;  aq. 
sol.  decomp.  on  boiling  giving  off  SO2  and 
forming  V2O4,  2H2O.  (Gain,  C.  R.  1906,  143. 
824.) 

Vanadyl  zinc  sulphite,  ZnO,  3VO2,  2SO2. 

Decomp.  slowly  in  the  air. 

Sal.  in  H2O  without  decomp.  (Koppel,  Z. 
anorg.  1903,  35.  183.) 

Ytterbium  sulphite,  Yb2(SO3)8+9H2O. 

Insol.  in  H2O.  (Cleve,  Z.  anorg.  1902,  32. 
143.) 


Yttrium  sulphite,  Y2(SO3)3+3H2O. 
SI.  sol.  in  H2O.    (Cleve.) 

Zinc  sulphite,  basic,  2ZnSO3,  3Zn(OH)2. 
(Seubert,  Arch.  Pharm.  229.  321.) 
ZnSO3,  Zn(OH)2+H2O.    (Seubert.) 

Zinc  sulphite,  ZnSO3+2,  and  2V2H2O. 

Very  si.  sol.  in  H2O.  100  pts.  H2O  dissolve 
0,16  pt.  ZnSO3+2H2O.  (Henston  and  Tich- 
borne,  Brit.  Med.  J.  1890.  1063.) 

Easily  sol.  in  H2SO3+Aq.    (Koene.) 

Sol.  in  NH4OH+Aq. 

Insol.  in  alcohol. 

Decomp.  into  basic  salt  by  boiling  H2O. 
(Seubert,  Arch.  Pharm.  229.  1.) 

Zinc  sulphite  ammonia,  ZnSO8,  NH8. 

Decomp.  by  H2O.  Sol.  in  NH4OH+Aq, 
(Rammelsberg,  Pogg.  67.  255.) 

Zirconium  sulphite. 

Insol.  in  H2O.  Somewhat  sol.  in  H2SO3-f 
Aq,  from  which  it  is  repptd.  on  boiling.  Sol. 
in  (NH4)2SO3+Aq,  from  which  Zr  hydroxide 
is  pptd.  on  boiling.  (Berzelius.) 

Zr(SO3)2+7H2O.  Ppt.  (Venable,  J.  Am. 
Chem.  Soc.  1895,  17.  449.) 

Sulphuryl  bromide,  S02Br2. 

(Odling,  Chem.  Soc.  7.  2.) 

Does  not  exist.      (Sestini,   Bull.   Soc.   10. 
226;  Melsens,  C.  R.  76.  92;  Michaelis.) 
' '  ^*i^BI^HHHp^*^'    ^^ 

Sulphuryl  chloride,  SO2C12. 

Decomp.  by  H2O  and  alcohol. 

Decomp.  by  moist  air,  water,  or  abs. 
alcohol;  more  rapidly  by  alkalies,  HC1,  SO2, 
etc.  '(Schiff,  A.  102.  111.) 

+H2O.  Only  si.  sol.  in  H2O  at  0°  with 
slow  decomp.  (Baeyer,  B.  1901,  34.  737.) 

-f-15H2O.  SI.  sol.  in  H2O  at  0°  and  stable 
therein  for  several  hours.  (Baeyer.) 

ZH'sulphuryl  chloride  (P?/rosulphuryl  chlor- 
ide), S2O6C12. 

Decomp.  slowly  with  H2O.  (Rose,  Pogg. 
44.  291.) 

Sol.  in  CC14  and  CHC18;  miscible  with 
h'quid  SO8. 

Sulphuryl  hydroxyl  chloride, 
SO3HC1=Q°SO2. 

Decomp.  on  moist  air,  and  violently  with 
H2O.  Not  miscible  with  CS2.  Decomp.  with 
alcohol. 

Sulphuryl   titanium  chloride,   SO8.   TiCl4  = 

TiCl3OSO2Cl. 

Slowly  deliquescent.  (Clausnitzer,  B.  11* 
2011.) 


1048 


SULPHURYL  CHLORIDE  STANNIC  OXYCHLORIDE 


ZH'sulphuryl  chloride  stannic  oxychloride, 

5S2O5C12,  4SnOCl2. 

Sol.  in  a  little  H2O,  but  decomp.  by  more 
H2O.  (Rose,  Pogg.  44.  320.) 

Sulphuryl  fluoride,  SO2F2. 

1  pt.  is  sol.  in  10  pts.  H2O  at  9°.  3  vol. 
are  sol.  in  1  vol.  alcohol  at  9°;insol.  in  cone. 
H2SO4  at  66°;  sol.  in  aq.  solution  of  KOH, 
Ca(OH)2,  Ba(OH)2  and  in  alcoholic  solution 
of  alkalies.  (Moissan,  C.  R.  1901,  132.  377.) 

Sulphuryl  hydroxyl  fluoride,  HSO»F. 

Violently  decomp.  by  H2O.  (Thorpe  and 
Kirwan,  Z.  anorg.  3.  63.) 

Sulphuryl  peroxide,  S04. 
See  Sulphur  heptoxide. 

Sulphydric  acid. 
See  Hydrogen  Sulphide. 

Sulphydroxyl. 
See  Sulphhydroxyl. 

Tantalic  acid,  H4Ta2O7  (?). 

Sol.  in  HF  (Rose),  and  KH3(C2O4)2+Aq 
(Gahn,  Schw.  J.  16.  437).  At  the  instant  of 
precipitation  is  sol.  in  various  acids.  (Rose.) 

Aluminum  tantalate. 

Insol.  in  H2O.    (Berzelius.) 

Ammonium    fozatantalate,   (NH4)tH7Ta7Oi9 

+H20. 
Somewhat, sol.  in  H2O.    (Rose,  Pogg.  102. 

57.) 

Barium  fozatantalate,  Ba4Ta8019+6H2O. 
SI.  sol.  in  H2O.    (Rose.) 

Cajsium  tantalate,  4Cs2O,  3Ta2O6+14H2O. 

Completely  sol.  in  a  small  amount  of  hot 
H2O.  (E.  F.  Smith,  J.  Am.  Chem.  Soc.  1908, 
30.  1666.) 

7Cs2O,  6Ta2O6+38H2O.  Pptd.  from  its 
aqueous  solution  by  alcohol.  (Smith.) 

Ferrous  tantalate,  Fe(TaO»)». 
Min.    Tantalite. 
5FeO,  4Ta2O6.    Min.  Tapiolite. 

Magnesium  ftezatantalate,  Mg4TaeOi»+ 
9H2O, 

Ppt.     (Rose,  Pogg.  102.  61.) 

4MgO,  Ta2O5.  Insol.  in  H2O.  (Joly,  C.  R. 
:81.  266.) 

Mercurous  tantalate,  5Hg2O,  4Ta2Q6-f-5H2O. 

Decomp.  by  warm  HNO3-f-Aq  (1.21  sp.  gr.) 
-with  separation  of  Ta2O5.  (Rose,  Pogg.  102. 


Potassium  tantalate,  KTaO8. 

Insol.  in  H2O.  Sol.  in  KOH+Aq.  (Marig- 
nac,  A.  ch.  (4)  9.  249.) 

Potassium  fcezatantalate,  K8Ta6O19+16H20. 
Sol.  without  decomp.  in  moderately  warm 
H2O.  Decomp.  by  boiling.  (Marignac,  A. 
ch.  (4)  9.  259.) 

Rubidium  tantalate,  4Rb2O,  3Ta2O5  +  14H2O. 
Sol.  in  H2O.  (E.  F.  Smith,  J.  Am.  Chem. 
Soc.  1908,  30.  1666.) 

Silver  tantalate,  4Ag2O,  3Ta2O6.. 

Completely  sol.  in  NH4OH+Aq.  HNO3+ 
Aq  dissolves  Ag2O,  and  Ta2Os  separates  out. 
(Rose,  Pogg.  102.  64.) 

Sodium  tantalate,  NaTaO8. 
Insol.  in  H2O.    (Rose.) 

Sodium  Aezatantalate,  Na8Ta6O19+25H2O. 

1  pt.  salt,  dissolves  in  493  pts.  H2O  at  13.5°, 
and  in  162  pts.  at  100°.  Very  slightly  sol.  in 
alcohol.  Insol.  in  alkaline  solutions.  (Rose.) 

Pertantalic  acid. 
See  Pertantalic  acid. 

Tantalum,  Ta. 

Not  attacked  by  HC1,  HNO3,  aqua  regia,  or 
hot  cone.  H2SO4.  Easily  sol.  in  a  mixture  of 
HNO3  and  HF  (Berzelius,  Pogg.  4.  6;  Rose). 
Also  sol.  in  HF  alone  (Berzelius.) 

Not  attacked  by  alkali  hydrates +Aq. 

Insol.  in  single  acids  and  in  aqua  regia. 
Oxidized  by  a  mixture  of  HF  and  aqua 
regia.  (Moissan,  C.  R.  1902,  134.  211.) 

Pure  Ta  is  insol.  in  boiling  H2SO4,  HNO8, 
HC1,  aqua  regia  or  mixtures  of  these  acids; 
slowly  sol.  in  HF-f  Aq.  (v.  Bolton,  Zeit. 
Elektrochem.  1905,  11.  45.) 

Tantalum  bromide,  TaBr6. 
Decomp.  by  H2O.    (Rose.) 


Tantalum  ^chloride,  TaCl2+2H2O. 

Sol.  in  H2O  when  freshly  prepared, 
brie",  C.  R.  1907,  144.  805.) 


(Cha- 


Tantalum  pewfczchloride,  TaCl6. 

Takes  up  H2O  from  the  air  without  deli- 
quescing. Decomp.  by  H2O.  Sol.  in  H2SO4. 
Sol.  in  cold  HCl-fAq  to  a  cloudy  liquid, 
which  gelatinises  after  a  time.  Not  com- 
pletely sol.  in  boiling  HCl+Aq,  and  the 
solution  does  not  gelatinise  by  the  subsequent 
addition  of  water,  but  all  goes  into  solution. 
Partly  sol.  in  KOH  +Aq.  Insol.  in  K2SO3+ 
Aq.  Sol.  in  absolute  alcohol. 


TELLURATE,  CAESIUM  HYDROGEN 


1049 


Tantalum  pentofluoride,  TaF6. 

Solubility  in  H2O. 

Very  hydroscopic;  sol.  in  H2O.     (Ruff,  B. 

•*  >r  _!_, 

1909,  42.  494.) 

Mols 

TT    (~\     4. 

MOlS 

H2TeO4 

Solid  phase 

Temp. 

% 

JC12U    tO 

Iw.^1 

to  100 

Tantalum  fluoride  with  MF. 

H2TeO4 

.  mol 
H2TeO4 

mols 
H  2O 

See  Fluotantalate,  M. 

Tantalum  hydroxide,  TaaO6,  zH,O. 

H2TeO4+6H2O 

tc 

0° 
5° 

13.92 

17.84 

66.2 
49.2 

1.51 
2.03 

See  Tantalic  acid. 

11 

10° 

26.21 

30.2 

3.31 

. 

tf 

15° 

32.79 

21.9 

4.55 

Tantalum  nitride,  TaN. 

H2TeO4.2H2O 

10° 

25.29 

31.7 

3.15 

Not  sol.  in  any  acids,  except  a  mixture  of 
HF   and   HNO3.      (Rose,    Pogg.    100.    146.) 

i 

18° 
30° 

28.90 
33.36 

26.2 
21.4 

3.82 
4.67 

Ta3N5.    (Joly,  Bull.  Soc.  (2)  26.  506.) 

t 

40° 
60° 

36.38 
43.67 

18.8 
14.2 

5.33 
7.04 

Tantalum  dioxide,  Ta2O2(?). 

1 

80° 

51.55 

10.07 

9.93 

Sol.   in  HF  with  evolution  of  hydrogen. 

i 

100° 

60.84 

6.89 

14.52 

(Hermann,  J.  pr.  (2)  6.  69.) 

(Mylius,  B.  1901,  34.  2211.) 

Tantalum  tefr-oxide,  Ta2O4. 

Not  attacked  by  any  acid,  not  even  a  mix- 
ture of  HNO3  and  HF.  (Berzelius,  Pogg.  4. 
20.) 

Decomp.  by  HC1.  (Smith,  Z.  anorg.  1894, 
7.  98.) 

Tantalum  pen toxide,  Taa08. 

Insol.  in  any  acid,  even  boiling  H2SO4  or  in 
HF.  (Berzelius.) 

Sol.  in  fused  KHSO4,,  10  pts.  being  necessary 
to  dissolve  1  pt.  Ta2O5. 

Tantalum  silicide,  TaSi2. 

Insol.  in  most  inorganic  acids.  Sol.  in 
HFandinHF+HNO3. 

Decomp.  by  fused  alkali  hydroxides.  (Hon- 
igschmid,  M.  1907,  28.  1027.) 

Tantalum  sulphide,  Ta2S4. 

Not  attacked  by  HCl+Aq.  Oxidised  by 
boiling  with  HNO3+Aq,-  more  rapidly  with 
aqua  regia.  Attacked  by  H2SO4  on  heating. 
Not  completely  sol.  in  HF  or  a  mixture  of  HF 
and  HN03. 

Telluretted  hydrogen,  TeH2. 
See  Hydrogen  telluride. 

Telluric  acid,  H2TeO4. 

Insol.  in  H2O,  cold  cone.  HC1,  hot  HNO3,  or 
boiling  KOH+Aq,  but  when  heated  with 
H2O  is  gradually  converted  into  H2TeO4+ 
2H2O  and  dissolved. 

+2H2O.  Very  slowly  sol.  in  cold  H2O,  but 
sol.  in  hot  H2O  in  every  proportion.  Insol 
in  absolute  alcohol;  sol.  in  dil.  alcohol  ac- 
cording to  the  amount  of  H2O  present.  Sol 
in  acids  and  alkalies.  Insol.  in  alcohol  or 

Insol.  in  alcohol;  sol.  in  NaOH+Aq 
(Mylius,  B.  1901,  34.  2216.) 

Stable  in  the  air. 

Sol.  in  H2O;  pptd.  by  HNO3.  (Stauden 
maier,  Z.  anorg.  1895, 10. 191.) 


+6H2O.  Obtained  from  solutions  at  0°. 
Staudenmaier,  Z.  anorg.  1895,  10.  191.) 

AKotelluric  acid,  H2TeO4. 

Miscible  with  H2O. 

Sol.  in  alcohol;  pptd.  by  NaOH+Aq  but 
sol.  in  excess.  (Mylius,  B.  1901,  34.  2216.) 

Tellurates. 

Neutral  alkali  salts  are  sol.  in  H2O;  the 
acid  salts  are  only  si.  sol.  therein,  but  dissolve 
in  HCl+Aq. 

Aluminum  tellurate. 

Ppt.  Sol.  in  excess  of  aluminum  salts  +Aq. 
(Berzelius.) 

Ammonium  tellurate,  (NH4)2TeO4. 

Slowly  but  completely  sol.  in  H2O.  SI.  sol. 
in  NH4OH+Aq  or  NH4Cl+Aq.  SI.  sol.  in 
alcohol.  (Berzelius.) 

(NH4)2O,  2TeO3.  SI.  sol.  in  H2O,  but  more 
sol.  than  the  corresponding  K  salt. 

(NH4)2O,  4TeO3.  Very  si.  sol.  in  H2O. 
Insol.  in  alcohol.  (Berzelius.) 

Barium  tellurate,  BaTeO4+3H2O. 

SI.  sol.  in  cold,  more  in  boiling  H2O.  Easily 
sol.  in  HNO3+Aq.  (Berzelius.) 

BaH2(TeO4)2+2H2O.  More  sol.  in  H2O 
than  BaTeO4.  Decomp.  by  H2O.  (Ber- 
zelius.) 

BaO,  41eO3.  More  sol.  in  H2O  than  either 
BaTeO4  or  BaH2(TeO4)2.  (Berzelius.) 

Bismuth  tellurate,  Bi2TeO8+2H8O. 

Min.  Montanite.  Sol.  in  HCl+Aq  with 
evolution  of  Cl. 

Cadmium  tellurate,  CdTeO4. 

Ppt.    Sol.  in  HCl+Aq.    (Oppenheim.) 

Caesium  hydrogen  tellurate,  CsHTeO4+ 

M>H20. 

1  pt.  is  sol.  in  30  pts.  H2O.  (Norris,  Am. 
Ch.  J.  1901,  26.  321.) 


1050 


TELLURATE,  CALCIUM 


Calcium  tellurate,  CaTeO4. 

Ppt.    Sol.  in  hot  H2O.     (BerzeliusV) 

Chromic  tellurate,  Cr2(TeO4)3. 
Ppt.    Sol.  in  excess  of  Cr  salts +Aq. 

Cobaltous  tellurate. 
Ppt.    (Berzelius.) 

Cupric  tellurate,  CuTeO4. 

Ppt.     (Berzelius.) 

CuO,  2TeO3.    Ppt.    (B.) 

Cu3TeO6.    Insol.  in  H2O. 

Sol.  in  HC1,  HNO3,.  NH4OH,  KCN  and 
acetic  acid.  (Hutchins,  J.  Am.  Chem.  Soc. 
1905,  27.  1181.) 

Glucinum  tellurate,  GlTeO4. 
Insol.  in  H2O. 

Iron  (ferrous)  tellurate,  FeTeO4. 
Ppt.    Min.  Ferrotellurate. 

Iron  (ferric)  tellurate,  Fe2(TeO4)3. 

Ppt.    Sol.  in  ferric  salts +Aq.    (Berzelius.) 

Lead  tellurate,  basic. 

Not  completely  insol.  in  H2O. 

Lead  tellurate,  PbTeO4. 

Somewhat  sol.  in  H2O. 

PbO,  2TeO3.    More  sol.  than  PbTeO4. 

PbO,  4TeO3.  SI.  sol.  in  H2O.  Sol.  in 
HNO3+Aq,  less  sol.  in  HC2H302+Aq.  (Ber- 
zelius.) 

Lithium  tellurate,  Li4TeO6+sH2O. 

SI.  sol.  in  H2O  with  decomp.  (Mylius,  B. 
1901,  34.  2209.) 

Magnesium  tellurate,  MgTeO4. 
Ppt.    More  sol.  in  H2O  than  the  Ba,  Sr.  or 

Ca  salts. 

MgTe2O7.    More  sol  in  H 2O  than  MgTeO4. 

Manganous  tellurate. 
Ppt. 

Mercurous  tellurate,  basic,  3Hg2O,  2Te03. 
Ppt.     (Hutchins,  J.  Am.  Chem.  Soc.  1905, 
27.  1178.) 

Mercurous  tellurate,  Hg2TeO4. 
Ppt.    Min.  Maqnolite. 

Mercuric  tellurate,  HgTe04. 

Ppt.  Very  easily  decomp.  by  H2O.  (Hut- 
chins,  J.  Am.  Chem.  Soc.  1905,  27.  1179.) 

+2H20.     Slowly  decomp.  by  cold  H2(X 

Rapidly  decomp.  by  boiling  H2O.  (Hut- 
chins.) 

Hg3TeO6.  Insol.  in  H2O.  Unchanged  by 
boiling  with  H2O. 


Sol.  in  HNO3,  but  more  readily  sol.  in  HC1. 
(Hutchins.) 

Mercuric  tellurate. 

Ppt.    (Berzelius.) 

Mercurous  hydrogen  tellurate,  HgHTeO4 

+3H2O. 

Stable  in  the  air  if  protected  from  the  light 
'Insol.  in  H2O.    Decomp.  by  boiling  H20  or 

by  an  excess  of  cold  cone.  HgNO3+Aq. 
Sol.  in  dil.  HNO3  or  dil.  acetic  acid.    (Hut- 

chins,  J.  Am.  Chem.  Soc.  1905,  27.  1177.) 

Nickel  tellurate. 
Ppt. 

Potassium  tellurate,  K2Te04+5H2O. 

Deliquesces.     Sol.  in  H2O.     Very  si.  sol. 
in  H2O  containing  KOH. 
100  g.  H20  dissolve  at: 

0°  20°  30° 

8  .  82        27  .  53        50  .  42  g.  K2TeO4. 
(Rosenheim  and  Weinheber,  Z.  anorg.  1911, 
69.  264.) 

Insol.  in  alcohol.    (Berzelius.) 

K2O;  2TeO3.  Insol.  in  H2O,  acids,  or 
alkalies.  (B). 

KHTeO4+HH2O.  SI.  sol.  in  cold,  more 
sol.  in  hot  H2O.  (Berzelius.) 

K2O,  3TeO3+5H2O.  Much  more  sol.  in 
hot  than  in  cold  H2O.  (Hutchins,  J.  Am. 
Chem.  Soc.  1905,  27.  1174.) 

K2O,  4TeO3.  Insol.  in  H2O,  HC1,  or  HNO3 
-fAq.  Sol.  by  long  heating  with  cone.  HNO3 
+Aq. 

KHTeO4,  H2TeO4+KH2O.-  SI.  sol.  in 
H20. 

Rubidium  tellurate,  Rb2TeO4  +3H2O  . 

Sol.  in  about  10  pts.  H2O.  (Norris,  Am. 
Ch.  J.  1901,  26.  322.) 

Rubidium  hydrogen  tellurate,  RbHTeO4 


Sol.  in  about  20  pts.  cold  H2O.  SI.  more 
sol.  in  hot  H2O.  (Norris,  Am.  Ch.  J.  1901, 
26.  320.) 

Silver  tellurate,  3Ag2O,  TeO8. 

Sol.  in  NH4OH+Aq. 

3Ag2O,    2TeO3.      Insol.    in    boiling    H2O. 

+3H2O.  Ppt.  Unchanged  by  cold  H2O. 
Gradually  decomp.  by  boiling  H2O.  (Hut- 
chins,  J.  Am.  Chem.  Soc.  1905,  27.  1169.) 

Ag2TeO4.  Decomp.  by  H2O  into  3Ag20, 
TeO3.  Sol.  in  NH4OH+Aq. 

+2H2O.  Insol.  in  hot  and  cold  H2O.  Sol. 
in  NH4OH,  KCN,  Na2S2O3,  HNO3,  H2SO4 
and  HC2H3O2+Aq.  Decomp.  by  cone.  HNO3 
H2SO4  or  acetic!  acid.  (Hutchins,  J.  Am. 
Chem.  Soc.  1905,  27.  1165.) 


TELLURIUM  CHLORIDE  SULPHUR  OXIDE 


1051 


Ag2TeO7.    Ppt. 
Ag2O.  4TeO3.    Ppt. 

Could  not  be  obtained.  (Hutchins,  J. 
Am.  Chem.  Soc.  1905,  27.  1168.) 

Sodium  tellurate,  Na2TeO4+2H2O. 

Very  si.  sol.  in  hot  or  cold  H2O.  When 
heated  to  drive  off  2H2O  becomes  insol.  in 
H2Q,  but  sol.  in  dil.  HNO3+Aq.  (Berzelius.) 

1  pt.  is  sol.  in  about  130  pts.  H2O  at  18°; 
50  pts.  H20  at  100°. 

+4H2O.  1  pt.  is  sol.  in  about  70  pts.  H2O 
at  18°;  40  pts.  H2O  at  50°.  (Mylius,  B.  1901, 
34.  2209.) 

Na2Te2O7  +4H2O  =  NaHTeO4  + 1  ^H2O . 
Slowly  but  completely  sol.  in  H2O.     SI.  sol. 
in  NaC2H3O2+Aq.    Insol.  in  alcohol.     (Ber- 
zelius.) 

Na2O,  4Te03.  Insol.  in  H2O,  acids,  or 
alkalies,  except  by  long  boiling  with  HNO3  + 
Aq. 

+zH2O.  (a)'  Slowly  sol.  in  H2O.  (/3) 
Insol.  even  in  boiling  H2O. 

Na4TeO5+8H2O.  Very  sol.  in  H2O  but 
with  decomp.  (Mylius.) 

Strontium  tellurates. 
Resemble  Ca  salts. 

Thallous  teUurate,  Tl2TeO4. 

SI.  sol.  in  H2O.  (Dennis.  J.  Am.  Chem. 
Soc.  1898,  18.  975.) 

Thorium  tellurate. 

Ppt.    Insol.  in  excess  of  thorium  salts  +Aq. 

Uranium  teUurate,  U2(Te4O)  3(?) . 

Ppt.     Insol.   in  H2O  or  UO2(NO3)2+Aq. 

Yttrium  teUurate. 

Ppt.    Insol.  in  H2O  or  Yt  salts +Aq. 

Zinc  teUurate,  Zn3TeO6. 

Insol.  in  H20. 

Sol.  in  HNO3,  HC1,  H2SO4  and  acetic  acid. 
(Hutchins,  J.  Am.  Chem.  Soc.  1905,  27.  1181.) 

• 

Zirconium  tellurate. 
Ppt.     (Berzelius.) 

Tellurium,  Te. 

Insol.  in  H2O  or  HCl+Aq.  SI.  sol.  in  hot 
cone.  H2SO4,  but  separates  out  on  cooling. 
Sol.  in  boiling  cone.  H2SO4.  Easily  oxidised 
by  HNO3  or  aqua  regia.  Sol.  in  boiling  very 
cone.  KOH+Aq,  separating  out  again  on 
cooling. 

Not  attacked  by  boiling  cone.  HNO3+Aq, 
according  to  Hartung-Schwartzkoff  (Ann. 
Min.  (4)  19.  345). 

Sol.  in  warm  cone.  KCN+Aq. 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  830.) 


100  pts.  methylene  iodide  dissolve  0.1  pt' 
Te  at  12°.  (Retgers,  Z.  anorg.  3.  343.) 

Ya,  com.  oleic  acid  dissolves  0.0014  g.  Te 
in  6  days.  (Gates,  J.  phys.  Ch.  1911,  15. 
143.) 

A  colloidal  solution  of  Te  in  H2O  can  be 
obtained.  It  exists  in  two  modifications, 
a  brown  and  a  blue-gray.  Both  can  be 
diluted  with  H2O  or  concentrated  by  boiling 
without  decomp.  They  are,  however,  de- 
comp. by  electrolytes,  especially  NH4G1. 
(Gutbier,  Z.  anorg.  1902,  32.  53.) 

TeUurium  cfabromide,  TeBr2. 

Decomp.  on  air  or  by  H2O.     (Rose,  Pogg. 

Cone,  tartaric  acid  dissolves  partly  with- 
out decomp.  (Brauner,  M.  1891,  12.  34.) 

TeUurium  tetrabromide,  TeBr4. 

Sol.  in  a  little,  but  decomp.  by  much  H2O. 

Completely  sol.  in  tartaric  acid+Aq  (1:1). 
(Brauner,  M.  1891,  12.  34.) 

TeUurium  hydrogen  >romide,  TeBr4,  HBr-f- 
5H2O. 

Fumes  in  the  air.  Deliquescent.  Stable 
in  an  atmos.  of  HBr.  (Metzner,  C.;  R.  1897, 

124.  1951.) 

TeUurium  ^'chloride,  TeCla., 

Decomp.  on  air,  or  by  H2O  or  HCl+Aq. 
(Ros-e,  Pogg.  21.443.) 

TeUurium  fctfrachloride,  TeCl<. 

Extremely  deliquescent.  Decomp.  by 
cold  H2O,  with  separation  of  oxychloride  and 
tellurous  acid.  Sol.  in  hot  H2O  with  decomp. 
Sol.  in  dil.  HC1  +Aq  without  decomp.  (Rose. 
Pogg.  21.  443.) 

Insol.  in  sulphur  chloride  and  in  CS2. 
(Lenher,  J.  Am.  Chem.  Soc.  1902,  24.  188.) 

TeUurium  hydrogen  chloride,  TeCl4,  HC1+ 
5H2O. 

Easily   decomp.      (Metzner.    C.   R.    1897, 

125.  £4.) 

TeUurium  chloride  with  MCI. 
See  Chlorotellurate,  M. 

TeUurium  fetfrachloride  ammonia, 
TeCl4,  3NH3. 

Decomp.  by  H2O.  (Metzner,  C.  R.  1897, 
124.  33.) 

TeCl4,  4NH3.  Not  deliquescent.  Decomp. 
by  H20.  (Espenschied,  J.  pr.  80.  480;) 

TeUurium  tefrachloride  sulphur  ^n'oxide,  x 

TeCl4,  S03. 

Ppt.     ((Prandtl,  Z.  anorg.  1909,  62.  247.) 
TeCl4,2SO3.     Decomp.  by  moisture.     On 

heating  at  120°,  it  gives  TeCl4,SO3.    (Prandtl.), 


1052 


TELLURIUM  FLUORIDE 


Tellurium  teJrafluoride,  TeF4. 
(Metzner,  C.  R.  1897,  126.  25.) 
+H2O.     (Hogbora,  Bull.  Soc.  (2)  35.  60.) 

Tellurium  Aezafluoride,  TeFfl. 

Decamp,  by  H2O  slowly  but  completely. 
(Prideaux,  Chem.  Soc.  1906,  39.  322.) 

Tellurium  zirconium  fluoride, 
See  Fluozirconate,  tellurium. 

Tellurium  diodide,  Telj. 

Insol.  in  H2O.    (Rose,  Pogg.  21.  443.) 

Tellurium  tefraiodide,  TeI4. 

Insol.  in  cold,  decomp.  by  hot  H20  or 
alcohol.  Sol.  in  HI,  but  only  sol.  in  MI  +  Aq. 
(Berzelius.) 

Data  on  solubility  of  TeI4  in  HI+I+Aq 
are  given  by  Menke  (Z.  anorg.  1912,  77.  283.) 

Tellurium  hydrogen   iodide,   TeI4,    HI+ 
8H2O,  and  +9H20. 

Deliquescent.  (Metzner,  A.  ch.  1898,  (7) 
16.  203.) 

Tellurium  nitride, 
Two  forms. 

a.  Stable  at  ord.  temp. 

b.  Unstable  at  ord.  temp. 

(Franz  Fischer,  B.  1910,  43.  1472.) 

TeN.  Not  attacked  by  H2O  or  dil.  acetic 

acid. 

Insol.  in  liquid  NH3.    Decomp.  by  KOH+ 

Aq.    (Metzner,  A.  ch.  1898,  (7)  16.  203.) 

Tellurium  monoxide,  TeO. 

SI.  sol.  in  cold  dil.  HC1  or  H2S04+Aq. 
Easily  oxidised  by  HN03+Aq  or  aqua  regia. 
Decomp.  immediately  by  boiling  cone.  HC1+ 
Aq.  Slowly  decomp.  by  KOH+Aq.  (Divers 
and  Shimose",  Chem.  Soc.  36.  563.) 

Tellurium  dioxide,  TeO2. 

Very  si.  sol.  in  H2O.  SI.  attacked  by  acids. 
SI.  sol.  in  NH4OH  or  alkali  carbonates  -f  Aq. 
Easily  sol.  in  NaOH  or  KOH+Aq.  Not  sol. 
in  less  than  150,000  pts.  H2O.  Easily  sol. 
in  warm  dil.  HNO8+Aq.  Sol.  in  warm 
H2SO4+Aq.  (Klein  and  Morel,  Bull.  Soc. 
(2)  43.  203.) 

20%  H2SO4+Aq.  dissolves  on  warming 
about  0.7%;  30%  H*SO4+Aq,  about  0.85%: 
50%  H2SO4+Aq,  about  4.4%. 

These  solutions  are  supersat.  and  TeO2 
separates  from  the  more  dil.  acids  on  stand- 
ing. (Brauner,  M.  1891,  12.  34.) 

Min.  Tellurite. 

Tellurium  dioxide  hydrobromic  acid,  TeOo 
3HBr. 

(Ditte,  C.  R.  83.  336.) 


Tellurium  dioxide  hydrochloric  acid,  TeO2, 

2HC1. 

(Ditte,  C.  R.  83.  336.) 
Te02,  3HC1.     (Ditte.) 


Tellurium  tfn'oxide,  TeO3. 

Insol.  in  cold  or  hot  H2O,  cold  HCl+Aq,  or 
cold  or  hot  HNO3-fAq.  Insol.  in  moderately 
cone.  KOH+Aq,  but,  when  the  KOH+Aq 
is  very  cone.,  is  sol.  if  boiling. 

Tellurium  oxide,  2TeO2,  TeO3. 
"  Tellurium  tellurate." 
(Metzner,  A.  ch.  1898,  (7)  16.  203.) 

Tellurium  oxybromide. 

Insol.  in  H2O.     (Ditte.  A.  ch.  (5)  10.  82.) 

Tellurium  oxybromide  sulphur  in'oxide, 
TeOBr2,  2SO3. 

Deliquescent.  (Prandtl,  Z.  anorg.  1909, 
62.  247.) 

Tellurium  oxychloride,  TeOCl2. 
Insol.  in  H2O.     (Ditte.) 

Tellurium  oxyfluoride,  TeF4,  TeO2+2H2O. 

Sol.  in  H2O  containing  HNO3.  Decomp. 
by  H2O. 

2TeF4,  3Te02+6H2O.  Decomp.  by  H2O. 
(Metzner,  C.  R.  1897,  125.  25.) 

Tellurium  sulphide,  TeS. 

Insol.  in  CS2;  very  unstable.  (Snelling, 
J.  Am.  Chem.  Soc.  1912,  34.  802.) 

Tellurium  di'sulphide,  TeS2. 

Insol.  in  H2O  or  dil.  acids.  Sol.  in  alkali 
hydrates  or  sulphides +Aq. 

CS2  dissolves  out  S,  so  that  the  substance 
is  probably  a  mixture.  (Becker,  A.  180.  257.) 

Tellurium  bisulphide,  TeS3. 

Insol.  in  H2O.    Sol.  in  K2S+Aq. 

Tellurium  sulphoxide,  Te&O8. 

Decomp.  by  H2O.  -  Sol.  in  H2SO4.  (Weber, 
J.  pr.  (2)  26.  218.) 

Is  tellurium  sulphite.  (Divers,  Chem. 
Soc.  49.  583.) 

Tellurous  acid,  H2TeO8. 

Appreciably  sol.  in  H2O  and  acids, 
in  alkali  hydrates  or  carbonates +Aq. 

Tellurites. 

The  neutral  and  acid  tellurites  of  the  alkali 
metals  are  sol.  in  H2O.  Ba,  Sr.  Ca,  and 
Mg  tellurites  are  si.  sol.,  and  the  other  salts 
yjsol.  in  H2O.  Most  tellurites  are  sol.  in 
-tld+Aq. 


TERBIUM 


ior>;t 


Aluminum  tellurite. 

Ppt.     Insol.  in  Al  salts +Aq.     (Berzelius.) 

Ammonium  tellurite,  (NH4)HTeO8,  H2TeO3+ 

3»/iHjO. 

Sol.  in  H2O,  from  which  it  is  precipitated 
by  NH4Cl+Aq  or  alcohol.  (Berzelius.) 

Barium  tellurite,  BaTe08. 

SI.  sol.  in  H2O  when  prepared  in  the  moist 
way.  (Berzelius.) 

BaO,  4TeO2. 

Cadmium  tellurite. 

Ppt.  Sol.inHNO3,andHCl+Aq.  (Oppen- 
heim.) 

Calcium  tellurite,  CaTeOa. 
SI.  sol.   in   cold,   more   sol.   in   hot  H2O. 

(Berzelius.) 
CaO,  4TeO2. 

Chromium  tellurite. 
Ppt.    Sol.  in  excess  of  chromic  salts  -fAq. 

Cobaltous  tellurite. 
Ppt. 

Cupric  tellurite. 
Insol.  in  H2O.    (Berzelius.) 

Glucinum  tellurite. 
Insol.  in  H2O. 

Indium  teUurite,  In2(TeO3,  2In(OH),. 
Ppt.     (Renz,  Dissert.  1902.) 

Ferrous  tellurite. 
Ppt. 

Ferric  tellurite. 
Ppt. 

Lead  tellurite,  PbTeO,. 

Ppt.    Easily  sol.  in  acids.    (Berzelius.) 

Lithium  tellurite,  Li2TeO,. 

Sol.  in  H2O.     (Berzelius.) 

LijO,  2TeOj.  Decomp.  by  cold  H,O  into 
LijTeOs  and  LijO,  4TeO4.  (B.) 

LijO,  4TeOj.  Sol.  in  hot,  much  less  in 
cold  H,0.  (B.) 

Magnesium  tellurite,  MgTeO*. 

Precipitate.  Much  more  sol.  in  HjO  than 
the  Ba,  Sr,  or  Ca  salt.  (Berzelius.) 

Manganous  tellurite. 
Ppt. 

Mercurous  tellurite.  . 

Ppt, 


Mercuric  tellurite. 
Ppt. 

Nickel  tellurite. 
Ppt. 

Potassium  tellurite,  K2TeO,. 

Not  deliquescent.  Slowly  sol.  in  cold. 
more  quickly  in  boiling  H2O.  (Berzelius.) 

K2O,  2TeOz.  Completely  sol.  in  boiling 
H2O,  from  which  K2O,4TeO2  crystallises.  (B.) 

K2O.  4TeO2+4H2O.  Decomp.  by  cold  HjO 
4nto  K2O,  TeO2,  and  K2O,  2TeO2,  which 
dissolve,  and  H2TeO3,  which  is  insol.  (B.) 

Potassium  Aezatellurite,  K20,  6TeO2+2H2O. 
Notdecomp.  by,  but  si.  sol.  in  JI2O.  (Klein 
and  Morel,  C.  R.  100.  1140.) 

SUver  tellurite,  Ag2TeO,. 
Ppt.     Sol.  in  NH4OH+Aq.     (Berzelius.) 
The  freshly  pptd.  salt  is  insol.  in  HjO;  sol. 

in  HNO3.  H2iSO4,  acetic  and  tartaric  and; 

decomp.  by  HC1.     (Lenher,  J.  Am.  Chem. 

Soc.  1913,  35.  727.) 
AgHTeOa.    Insol.  in  HjO.    Sol.  in  HNO8 

+Aq.    (Rose,  Pogg.  18.  60.) 

Sodium  tellurite,  NaaTeO,. 
Slowly  sol.  in  cold,  more  quickly  in  hot 
Precipitated  from   aqueous  solution 
by  alcohol.    (Berzelius.) 

Na2O,  2TeOs.  Decomp.  by  H/>  as  K  salt. 
(B.) 

,  4TeO2+5HjO.    As  above.    (B.) 


Strontium  tellurite,  SrTeO». 

Resembles  Ba  salt. 

SrHtlWV     Very  sL  sol.  in  H»O,  more 
easily  in  HNOa+Aq. 

Thorium  tellurite* 
Precipitate.   Insol.  in  HjO  or  Th  salto+Aq. 

Stannous  tellurite. 

Pptd.     in  presence  of  60,000  pte.     HjO. 
(Fischer.) 

Uranium  teHwite,  U,(TeO,)^ 
Ppt.    InsoL  in  U  salte+Aq. 

Yttrium  teUurite. 
Precipitate. 

lurite. 


Ppt. 


Ppt. 

Terbium,  *H>. 

Metal  baa  not  been  isolated. 

Has  been  decomp.  into  two  or  more  ele- 
ments by  Krttas  (Z.  anorg.  4. 27). 


1054 


TERBIUM  CHLORIDE 


Terbium  chloride,  TbCl3-f-6H2O. 

Sol.  in  H2O;  very  hydroscopic;  sol.  in  al- 
cohol.    (Urbain,  C.  R.  1908,  146.  128.) 

Terbium  hydroxide. 

Sol.    in    dilute    acids.      Decomposes    NH4 
salts  +Aq. 

Terbium  oxide,  T2O3. 

Sol.  in  dil.  acids,  even  after  ignition. 

Terbium  peroxide,  Tb407. 

Sol.  in  HNO3  and  in  hot  HC1.     (Urbain, 
C.  R.  1907,  146.  127.) 

Tetramine  chromium  compounds. 

See— 

Bromotetramine  chromium  compounds. 
Chlorotetramine  chromium  compounds. 
lodotetramine  chromium  compounds. 

Tetramine  cobaltic  compounds, 


See— 

Bromotetramine  cobaltic  compounds. 
Carbonatotetramine    cobaltic    compounds. 
Chlorotetramine  cobaltic  compounds. 
Croceocobaltic  compounds. 
Fuscocobaltic  compounds. 
Flavocobaltic  compounds. 
lodotetramine   cobaltic   compounds. 
Nitratotetramine  cobaltic  compounds. 
Praseocobaltic  compounds. 
Roseotetramine   cobaltic   compounds.  ~"; 
Sulphatotetramine  cobaltic  compounds. 
See  also  under  octamine  cobaltic  saltslfor 
many  tetramine  salts  as  yet  unclassified.  "" 

Tetramine  cobaltic  nitrite  with  MNO2, 

Co,(NH,)4(NO,).,  2MN02. 
See  Diamine  cobaltic  nitrite. 

Tetrathionic  acid,  H2S4O6. 

Known  only  in  aqueous  solution. 

Dil.  solution  can  be  boiled  without  decomp. 
Cone,  solution  decomp.  by  boiling. 

Addition  of  H2SO4  or  HC1  makes  solution 
more  stable.  (Fordos  and  Gelis,  C.  R.  15. 
920.) 

Tetrathionates. 

Tetrathionates  are  all  easily  sol.  in  H2O, 
but  insol.  in  alcohol 

Barium  tetrathionate,  BaS4O6-f2H2O. 

Very  sol.  in  H2O,  but  precipitated  by  addi- 
tion of  alcohol 

Cadmium  tetrathionate. 

Deliquescent.  Solution  in  H2O  gradually 
decomposes.  (Kessler,  Pogg.  74.  249.) 


Caesium  tetrathionate,  Cs2S4O6. 
(J.  Meyer,  B.  1907,  40.  1361.) 

Cuprous  tetrathionate,  Cu2S4O6. 

Decomp.  by  H2O.  (Chancel  and  Diacon, 
C.R.  1863,  56.  711.) 

Cupric  tetrathionate,  CuS4Oe. 

Sol.  in  H2O. 

Decomp.  by  long  boiling.  (Curtius  and 
Henkel,  J.  pr.  1888,  (2)  37.  148.) 

Lead  tetrathionate,  PbS4O6+2H2O. 
Sol.  in  H2O. 

Manganous  hydrogen  tetrathionate, 

MnH2(S406)2. 

Deliquescent.  Very  sol.  in  H2O  and  al- 
cohol. (Curtius  and  Henkel,  J.  pr.  (2)  37. 
148.) 

Nickel  tetrathionate  ammonia,  NiS4O6,  6NH3. 
Ppt.    Decomp.  by  H2O.    Insol.  in  alcohol. 
(Ephraim,  B.  1913,  46.  3109.) 

Potassium  tetrathionate,  K2S4O6. 

Soluble  in  H2O.    Insol.  in  alcohol. 

Difficultly  sol.  in  H2O.  (Kessler,  Pogg. 
1847,  74.  254.) 

Rubidium  tetrathionate,  Rb2S4O6. 

Not  hydroscopic.  (J.  Meyer,  B.  1907,  40. 
1356.) 

Sodium  tetrathionate,  Na2S4O6. 

Sol.  in  H2O.  Precipitated  therefrom  by 
a  great  excess  of  alcohol.  (Kessler,  J.  pr.  96. 
13.) 

+2H2O.     (Berthelot,  A.  ch.  (6)  17.  450.) 

Strontium  tetrathionate,  SrS406+6H2O. 
Sol.  in  H2O.  (Kessler,  Pogg.  74.  255.) 
More  sol.  in  H2O  than  Ba  salt. 

Zinc  tetrathionate. 

Sol.inH2O.    (Fordos  and  Gelis.) 

Zinc  hydrogen  tetrathionate,  ZnH2(S4O6)2. 

Extremely  sol.  in  H2O  and  alcohol.  (Cur- 
tius and  Henkel,  J.  pr.  (2)  37.  147.) 

Zinc  tetrathionate  ammonia,  ZnS4O6,  3NH3. 
Ppt.    (Ephraim,  B.  1915,  48.  641.) 

Thallic  acid. 

Potassium  thallate. 

Known  only  in  aqueous  solution.  (Car- 
stanjen,  J.  pr.  101.  55.) 

Does  not  exist.  (Lepsius,  Chem.  Ztg.  1890, 
1327.) 


THALLOUS  CHLORIDE 


1055 


Thallium,  Tl. 

Not  attacked  by  pure  H2O.  Easily  sol.  in 
dil.  H2SO4  or  HNO3+Aq.  Difficultly  sol. 
in  HCl+Aq.  Absolute  alcohol  dissolves 
considerable  quantity  in  a  short  time,  also 
methyl  alcohol,  and  acetic  ether.  (Bottger.) 

Not  easily  attacked  by  HF+Aq.  (Kiihl- 
mann.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  830.) 

l/z  ccm.  oleic  acid  dissolves  0.0424  g.  Tl  in 
6  days.  (Gates,  J.  phys.  Chem.  1911, 15. 143.) 

Thallium  arsenide,  TIAs. 

Decomp.  by  H2SO4.     (Carstanjen.) 

Thallous  azoimide,  T1N3. 

SI.  sol.  in  H2O. 

0.1712  pt.  is  sol.  in  100  pts.  H2O  at  0°; 

0.1965  pt.  is  sol.  in  100  pts.  H2O  at  5°; 

0.3  pt.  is  sol.  in  100  pts.  H2O  at  16°. 

Insol.  in  abs.  alcohol  and  ether. 

(Curtius,  J.  pr.  1898,  (2)  58.  284.) 
Thallothallic    azoimide,    T1N3,    T1N9. 

Explosive.  Decomp.  bv  hot  H2O  and  by 
acids.  (Dennis,  J.  Am.  Chem.  Soc.  1896,  18. 
973.) 

Thallous  bromide,  TIBr. 

Nearly  insol.  in  cold,  si.  sol.  in  boiling 
H2O.  (Willm,  Bull.  Soc.  (2)  2.  89.) 

1  1.  H2O  dissolves  0.00869  g.  mol.  TIBr  at 
68.5°.  (Noyes,  Z.  phys.  Ch.  6.  248.) 

SI  sol.  in  H2O.  0.48  X  10~2  g.  is  dissolved  in 
a  liter  of  sat.  solution  at  20°.  (Bottger,  Z. 
phys.  Ch.  1903,  46.  603.) 

1  1.  H2O  dissolves  420  mg.  TIBr  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  1904,  50.  356.) 

238  mg.  TIBr  are  contained  in  1  1.  sat. 
solution  at  0.13°;  289  mg.  at  9.37°;  423  mg. 
at  18°;  579  mg.  at  25.68°.  (Kohlrausch,  Z. 
phys.  Ch.  1908,  64.  168.) 

Solubility  of  TIBr  in  T1(NO3)  +Aq  at  68.5°. 


g.  mola.  per  1. 

g.  mols.  per  1. 

TINOs 

TIBr 

TiNOs 

TIBr 

0 

0.0163 
0.0294 
0.0955 

0.00869 
0.00410 
0.00289 
0.00148 

0 
4.336 
7.820 
25.400 

2.469 
1.164 
0.821 
0.420 

(Noyes,  Z.  phys.  Ch.  1890,  6.  248.) 

Insol.  in  acetone  (Naumann,  B.  1904,  37. 
4329) ;  pyridine  (Naumann,  B.  1904, 37. 4610) ; 
acetone  (Eidmann,  C.  C.  1899,  II.  1014). 

Thallic  bromide,  TlBr3. 

Deliquescent.  Easily  sol.  in  H2O  and 
alcohol.  (Willm.) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

+H2O.      Very    unstable.      Sol.    in    H2O, 


alcohol  and  ether.     (Meyer,  Z.  anorg.  1900, 
24.  353.) 

+4H2O.  Very  sol.  in  H2O.  (Thomas, 
C.  R.  1902,  134.  546.) 

Thallothallic  bromide,  TIBr,  TlBr3. 

Decomp.  by  H2O.  (Mever,  Z.  anorg.  1900, 
24.  354.) 

STIBr,  TlBr3.  Decomp.  by  H2O  into  TIBr 
and  TlBr3. 

Thallic  hydrogen  bromide,  TlBr3,  HBr. 

Very  sol.  in  H2O.  (Thomas,  C.  R.  1902, 
134.  546.) 

Thallic  bromide  ammonia,  TlBrs,  3NH3. 

Decomp.  by  H2O. 
Thallium  bromochloride,  TIClBr. 

Decomp.  by  H2O.  (Thomas,  C.  R.  1901, 
132.  1489.)  "  . 

TlClBr2+4H2O.    Ppt. 

TlCl2Br+4H2O.  Ppt.  Decomp.  by  H2O. 
(Thomas,  C.  R.  1902,  134.  546.) 

Tl3Cl2Br4.  Decomp.  by  H2O,  H2SO4  or 
HNO3.  (Thomas,  C.  R.  1900,  131.  894; 
C.  R.  1901,  132.  1489.) 

Tl4Cl3Br3.  Sol.  in  H2O.  (Thomas,  C.  R. 
1901,  132.  82.) 

TlClBr2,  3T1C1.  Cryst.  from  H2O  con- 
taining HNO3.  (Cushmann,  Am.  Ch.  J. 
1900,  24.  222.) 

T1C13,  3TlBr.  Sol.  in  H2O  without  decomp. 
(Cushmann.) 

"TlBrs',  3T1C1.     Decomp.  by  H2O.     (Cush- 
mann.) 

TlBr3,  TlCl.  Sol.  in  H2O  with  decomp. 
(Cushmann.) 

TlCls,  2TlBr,  11C1.  Sol.  in  H2O.  (Meyer, 
Z.  anorg.  1900,  24..  355-360.) 

TlBrs,   2T1C1,   TIBr.     Ppt.     Decomp.   by 


2(TlBr3,     TIBr).       Ppt. 

(Meyer.) 

2(T1C13,  TlCl),  (TlBrs,  TIBr).     Ppt.     De- 
comp, by  hot  H2O.    (Meyer.) 

Thallium  bromofluoride,  TlFBr2. 
Decomp.  in  moist  air. 
Sol.  in  abs.  alcohol.     (Gewecke,  A.  1909, 
366.  233.) 
Thallium  bromofluoride  ammonia, 

TlFBf2,4NH3. 
Decomp.  by  moisture. 
Difficultly  sol.  in  abs.  alcohol.     (Gewecke, 
AM909,  366.  234.) 
Thallous  chloride,  TlCl. 

Solubility  in  pts.  H2O  at  t°,  according  to 
H=Hebberling;  C  =  Crookes;  L  =  Lamy. 

0°        15°         16°       16.5° 
504      283.4      377        359  pts.  H2O, 
H  C  H          H 


100P 

about  50 
L 


100° 

52  .  5 

C 


100° 

63  pts.  H2O. 

H 


1056 


THALLOUS  CHLORIDE 


1  1.  H2O  dissolves  0.0161  g.  mol.  T1C1  at 
25°.  (Noyes,  Z.  phys.  Ch.  6.  249.) 

3.26  X 10  2  grams  are  dissolved  in  1  liter 
of  sat.  solution  at  20°.     (Bottger,  Z.  phvs. 
Ch.  1903,  46.  603.) 

1  1.  H2O  at  25°  dissolves  0.01606  g.  mol. 
T1C1.  (Geffcken,  Z.  phys.  Ch.  1904,  49.  296.) 

Solubility  in  H2O  at  t°. 
100  cc.  sat.  solution  contain  at: 
t°  0°        10°      20°      30°      40°      50° 

g.  T1C1   0.17    0.24    0.34   0.46    0.60    0.80 

t°  60°      70       80°      90°      99.3° 

g.  T1C1     1.02     1.29    1.60     1.97   2.41 
(Berkeley,  Trans.  Roy.  Soc.  1904,  203,  A, 
208.) 

1  1.  H2O  dissolves  3.040  T1C1  at  18°. 
(Kohlrausch,  Z.  phys.  Ch.  .1904,  50.  356.) 

2.27  g.  are  dissolved  in  1  1.  of  sat.  solution 
at  9.54°;  3.05  g.  at  17.7°;  3.97  g.  at  25.76°. 
(Kohlrausch,  Z.  phys.  Ch.  1908/64.  168.) 

0.01629  mol.  is  sol.  in  1  1.  H20  at  25°. 
(Hill,  J.  Am.  Chem.  Soc.  1910,  32.  1385.) 

0.01607  g.  equiv.  is  sol.  in  1  1.  H2O  at  25°. 
(Bray  and  Winninghoff,  J.  Am.  Chem.  Soc. 
1911,  33.  1665.) 

Much  less  sol.  in  H2O  containing  HC1  or 
HN03. 

Solubility  in  HCl+Aq  at  25°.    1  1.  dissolves 
g.  mol.  T1C1. 


g.  HCl 
added 

T1C1 

g.  HCl 
added 

T1C1 

0 

0.0283 
0.0560 

0.01610 
0.00836 
0.00565 

0.1468 
1.000 

0.00316 
0.00200 

(Noyes,  Z.  phys.  Ch.  6.  249.) 
Solubility  in  HCl+Aq.  at  25°. 


Concentration  of  HCl, 
equivalents  per  liter 


0 

0.025 

0.05 

0.10 

0.20 


Solubility  of  T1C1, 
equivalents  per  liter 


0.01612 
0.00869 
0.00585 
0.00384 
0.00254 


(Noyes,  Z.  phys.  Ch.  1892,  9.  614.) 
Solubility  in  HNO3+Aq  at  25°. 


Normality 
HNOs 


0.000 

0.4977 

1.0046 

2.0452 

4.017 


Sp.  gr.  of  the 
solution 


0.996 
1.0184 
1.0359 
1.0705 
1 . 1362 


g.  T1C1  dis- 
solved per  1. 


3.952 
5.937 
6.883 
8.143 
9.926 


(Hill  and  Simmons,  Z.  phys.  Ch.  1909,  67. 
605.) 


Concentration  of   KNOs 
milliequivalents  per  1. 

Solubility  of  TIC1. 
milliequivalents  per  1. 

10 
20 
50 
100 
300 
1000 

16.07 
17.16 
18.26 
19.61 
23.13 
30.72 

Nearly  insol.  in  NH4OH+Aq. 

More  sol.  in  K2CO3+Aq  than  in  H2O. 
3.86  g.  T1C1  are  sol.  in  1 1.  H2O  at  25°.  21.84  g. 
T1C1  are  sol.  in  1  1.  5N-K2CO3+Aq  at  25°. 
(Spencer  and  Le  Pla,  C.  C.  1908,  II.  198.) 


Solubility  in  KNO3+Aq  at  25°. 


(Bray  and  Winninghoff,  J.  Am.  Chem.  Soc. 
1911,  33.  1670.) 


Solubility  in  K2SO4+Aq  at  25°. 


Concentration  of  K2SO-i 
milliequivalents  per  1. 


10 

20 

50 

100 

300 

1000 


Solubility  of  T1C1 
milliequivalents  per  1. 


16.07 
17.79 
19.42 
21.37 
26.00 
34.16 


(Bray  and  Winninghoff,  J.  Am.  Chem.  Soc, 
1911,  33.  1670.) 


Solubility  in  Tl2SO4+Aq  at  25°. 


Concentration  of  TlnSCi 
milliequivalents  per  1. 

Solubility  of  T1C1 
milliequivalents  per  I. 

10 
20 
50 

1±          100 

16.07 
10.34 
6.77 
4.68 

(Bray  and  Winninghoff,  J.  Am.  Chem.  Soc. 
1911,  33.  1670.) 


Solubility  of  T1C1  in  salts +Aq  at  25°. 


Salt 

Concentration  of 
salt  g.  equiv.  per  1. 

T1C1  dissolved 
g.  equiv.  per  1. 

NH4C1 

-      0.025 
0.05 
0.2 

0.00872 
0.00593 
0.00271 

CaCl2 

0.025 
0.05 
0.10 
0.20 

0.00899 
0.00624 
0.00417 
0.00284 

THALLIUM  TUNGSTEN  CHLORIDE 


1057 


Solubility   of   T1C1  in   salts  +Aq 
Continued. 

at   25°.— 

Solubility  of  T1C1  in  HC2H3O2+Aq  at  25°, 
(g.  equiv.  per  1.) 

Salt 

Concentration  of 
salt  g.  equiv.  per  1 

T1C1  dissolved 
g.  equiv.  per  1. 

Acid                                      T1C1 

0.000                            0.01629 
0.5134                           0.01580 
1.013                             0.01495 
2.016                             0.0132 
4.180                             0.0099 
8.130                             0.0054 
11.49                               0.0026 
14.31                               0.0012 
16.01                               0.0005 

CdCl2 

0.025 
0.05 
0.10 
0.20 

OOOO 

01040 
0078 
00578 
00425 

CuCl2 

0.025 
0.05 
0.10 
0.20 

oooo 

00905 
00614 
00422 
00291 

(Hill,  J.  Am.  Chem.  Soc.  1910,  32.  1189.) 

Insol.  in  pyridine.  (Naumann,  B.  1904,  37. 
4610);    acetone.      (Naumann,    B.    1904,    37. 
4329.) 

Thallic  chloride,  T1C13. 

Anhydrous. 
Easily  sol.  in  H2O  and  in  most  ord.  sol- 
vents. 
In  contact  with  moist  air,  it  rapidly  be- 
comes hvdrated.     (Thomas,  C.  R.  1902   136. 
1053.) 
Difficultly  sol.  in  methyl  acetate.     (Nau- 
mann, B.  1909,  42.  3790.) 
Very  sol.  in  acetone.     (Renz,  B.  1902,  35. 
1110.) 
Difficultly  sol.  in  acetone.     (Naumann,  B. 
1904,  37.  4328.) 
+H2O.    Deliquescent,  and  very  easily  sol. 
inH2O.    (Werther.) 
Deliquescent,  and  very  easilv  sol.  in  H2O. 
(Werther.) 
-f  4H2O.    86.2  pts.  are  sol.  in  100  pts.  H2O 
at  17°.    Sp.  gr.  of  sat.  aq.  solution  at  17°  = 
1.85.    (Thomas,  C.  R.  1902,  136.  1052.) 
Very    hydroscopic.       (Meyer,    Z.    anorg. 
1900,  24.  336.) 
Very  sol.  in  alcohol  and  ether.    (Meyer,  Z. 
anorg.  1900,  24.  338.) 
+7^H2O.    Deliquescent.    (Werther.) 

MgCl2 

0.025 
0.05 
0.10 
0.20 

oooo 

00904 
00618 
00413 
00275 

MnCl2 

0.025 
0.05 
0.10 
0.20 

oooo 

00898 
00617 
00412 

00286 

KC1 

0.025 
0.05 
0.1 
.    0.2 

oooo 

00872 
00593 
00399 
00265 

NaCl 

0.025 
0.05 
0.10 

0.20 

0. 
0. 
0. 
0. 

00869 
00592 
00395 
00271 

ZnCl2 

0.025 
v-  0.05 
0.10 
0.20 

oooo 

00899 
00627 
00412 
00281 

T1C1O3 

0.025 

0. 

00897 

T1NO3 

0.025 
0.05 
0.10 

pop 

00883 
00626 
00423 

(Noyes,  Z.  phys.  Ch.  1892,  9.  609.) 


Solubility  of  T1C1  in  salts  -f  Aq  at  25°. 


Salt 

Mols  T1C1  sol.  in  1  liter  of 

O.5-N 

solution 

N 
solution 

2-N 
solution 

3-N 

solution 

4-N 
solution 

NH4NO3 
KNOs 
NaNOs 
LiNOs 
KClOa 
NaClOs 

0.02587 
0.02566 
0  .  02564 
0.02542 
0  .  02370 
0  02320 

0.03121 
0.03077 
0  .  03054 
0.03035 

0  .  02687 

0.03966 
0.03904 
0.03851 
0.03785 

0  .  03060 

0  .  04544 
0.04438 

0.03303 

0.05128 
0  .  03850 

(Geffcken,  Z  phys.  Ch.  1904,  49.  295.) 

Insol.     in     alcohol.     Easily    sol.    in    hot 
HgCl2+Aq.     (Carstanjen.) 


Thallothallic  chloride,  3T1C1,  T1C18. 

1  pi.  dissolves  in  pts.  H2O  at  t°,  according 
to  C=Crookes;  H  =  Hebberling;  L  =  Lamy. 

15°        17°       100°          100° 
380.1      346      52.9        20-25  pts.  H2O. 
C  H        C  L 

SI.    decomp.    by    dissolving.      (Lamy.) 

Thallic    hydrogen    chloride,    T1C18,    HC1+ 
3H20. 

Very  hygroscopic. 

Decomp.  by  H2O.    (Meyer,  Z.  anorg.  1900, 
24.  337.) 

Thallium  tungsten  chloride,  T1SW2C19. 

Nearly  insol.  in  H2O. 

Sol.  in  a  hot  mixture  of  equal  pts.  H2O  and 
cone.  HC1. 


1058 


THALLIC  ZINC  CHLORIDE 


SI.  sol.  in  cone.  HC1. 

Solubility  of  T1OH  in  H2O  at  t°. 

Nearly   insol.    in   most   organic   solvents. 
(Olsson,  B.  1913,  46.  575.) 

t° 

g.  equiv. 
1  1OH  per  1 

Sp.  gr.  15°/4° 

1       1  C1 

1     9Q1 

ThaUic  zinc  chloride,  2T1C13,  ZnCl2+6H2O. 

18.5 

i  .  i  ')  i 

1.554 

J-  .  _•  )  1 

1.317 

Can  be  cryst.  from  H2O.     (Gewecke,  A. 

19.5 

1.582 

1.322 

1909,  366.  224.) 

29 

1.803 

1.342 

23.1 

1.861  . 

1.377 

Thallic  chloride  ammonia,  T1C18,  3NH,. 

33.1 
36 

1.967 
2.075 

1.400 
1.417 

Decomp.  by  H2O.  Sol.  in  HCl+Aq  (Willm.) 

40 

2.240 

1.446 

44.5 

2.442 

. 

Thallium  chlorofluoride,  T1FC12. 

54.1 
59.4 

2.940 
3.281 

Very  hydroscopic. 

64.6 

3.601 

Decomp.  by  moist  air. 

78.5 

4.673 

Easily  sol.  in  abs.  alcohol.     (Gewecke,  A. 

90.0 

5.705 

1909,  366.  230.) 

99.2 

6.708 

+3H2O.    Not  hydroscopic. 
Decomp.    by    H2O,    alcohol    and    ether. 

(Bahr,  Z.  anorg.  1911.  71.  87.) 

(Gewecke.) 

Thallium  chlorofluoride  ammonia,  T1FC12, 
4NH3. 

Decomp.  by  H2O. 

Difficultly  sol.  in  abs.  alcohol  and  in  ether. 
(Gewecke,  A.  1909,  366.  232.) 

Thallium  chlorofluoride  potassium  chloride, 

2T1FCU,  KC1. 
Ppt.    (Gewecke,  A.  1909,  366.  231.) 

Thallous  fluoride,  T1F. 

Sol.  in  1%  pis.  H2O  at  15°,  and  in  much 
less  hot  H2O.  Difficultly  sol.  in  alcohol. 
(Buchner,  W.  A.  B.  62.  2.  644.) 

Deliquescent.    (Willm.) 


ThaUic  fluoride,  T1F8. 

Insol.  in  H2O  and  cold  HCl+Aq.    (Willm.) 
Cannot  be  obtained  in  pure  state.     (Ge- 

wecke, A.  1909,  366.  218.) 

Thallous  hydrogen  fluoride,  T1F,  HF. 
Sol.  in  1  pt.  H2O.    (Buchner.) 

Thallous  tungstyl  fluoride, 
See  Fluoxytungstate,  thallous. 

Thallous  vanadium  fluoride. 
See  Fluovanadate,  thallous. 

Thallous  vanadyl  fluoride. 
See  Fluozyvanadate,  thallous. 

Thallous  hydroxide,  T1OH. 
Sol.  in  H2O  and  alcohol. 


The  solubility  of  T12O  in  H2O   at  these 
temperatures  is  the  same  as  that  of  T1OH. 
+H2O.    (Willm,  Bull.  Soc.  (2)  6.  354.) 

ThaUic  hydroxide,  T12O3,  H2O=T1O(OH). 

Insol.  in  H2O.  Sol.  in  dil.  acids  and  am- 
monium salts  +Aq.  Insol.  in  caustic  alkali 
solutions. 

T1(OH),.  Easily  sol.  in  dil.  HC1  or  H2SO4 
+Aq.  (Carnegie,  C.  N.  60.  113.) 

Thallous  iodide,  Til. 

Very  si.  sol.  in  H2O. 

1  pt.  Til  is  sol.  in  pts.  H2O  at  t°.  C  =  ac- 
cording to  Crookes;  H  =  according  to  Hebber- 
ling;  L  =  according  to  Lamy;  W  =  according 
to  Werther. 

35°      15°,     16°      16-17°    19.4° 
20,0004450  16,000  11,676   14,654  pts.  H20, 

W         C        L          H          W 

20°       23.4°       45°     100°    100° 
11,954    10,482    5407    842     804  pts.  H2O. 
W          W          W        C        -H 

Sol.  in  17,000  pts.  H2O  at  20°.  (Long,  Z. 
anal.  30.  342.) 

Sat.  solution  at  20.15°  contains  63.6  mg. 
or  1.92X10  4  g.  mol.  Til  per  1.  (Bottger,  Z. 
phys.  Ch.  1903,  46.  603.) 

1  1.  H2O  dissolves  "56  mg.  Til  at  18°. 
(Kohlrausch,  2.  phys.  Ch.  1904,  60.  356.) 

36.2  mg.  are  dissolved  in  1 1.  of  sat.  solution 
at  9.90°;  56  mg.  at  18.1°;  84.7  mg.  at  26°. 
(Kohlrausch,  Z.  phys.  Ch.  1908,  64.  168.) 

Solubility  in  H2O  at  25°  =  1.76X104  mol. 
per  litre.  (Spencer,  Z.  phys.  Ch.  1912,  80. 

Not  decomp.  by  dil.  H2SO4,  HC1.  or  alkalies 
+Aq.  Decomp.  by  hot  dil.  HNO3+Aq,  and 
cold  cone.  HNO3.  Sol.  in  aqua  regia. 

Also  less  sol.  in  acetic  acid  than  in  H20. 
(Carstanjen.) 


THALLIUM  TELLURIDE 


1059 


Insol.  in  NH4OH+Aq.  (Werther.)  Not 
wholly  insol.  in  NH4OH+Aq.  and  solubility 
is  increased  by  presence  of  (NH4)2SO4  or 
NH4C1.  (Baubigny,  C.  R.  113.  544.) 

Sol.  in  13,000  pts.  NH4OH+Aq  (6^  or 
NH3).  Sol.  in  17,000  pts.  NH4OH+Aq 
1NH3).  (Long.) 

Insol.  in  dil.  KI+Aq  (1%  KI).  (Bau- 
bigny.) 

Much  more  insol.  in  KI+Aq  than  in  H20; 
1  pt.  dissolves  in  75,000  pts.  dil.  KI+Aq. 
(Lamy.) 

Nearly  insol.  in  Na2S2O3+Aq,  and  abso- 
lutely insol.  therein  in  presence  of  Pb  salts. 
(Werner.  C.  N.  63.  51.) 

Sol.  in  56,335  pts.  85%  alcohol  at  13°. 
(Werther.)  Sol.  in  18,934  pts.  98%  alcohol 
at  19°.  (Hebberling.) 

When  Til  is  shaken  with  alcohol  of  78°B 
(1  vol.  H2O+3  vols.  98%  alcohol)  at  22°,  and 
let  stand  with  Til  for  24  hours,  and  then 
evaporated  to  Vs  vol.,  there  is  shown  no  ppt. 
by  NH4SH+Aq.  (Baubigny.) 

Sol.  in  260,000  pts.  90%  alcohol,  and 
37,003  pts.  50%  alcohol  at  20°.  (Long.) 

Insol.  in  methylene  iodide.  (Retgers,  Z. 
anorg.  3.  343.) 

Insol.  in  acetone.  (Naumann,  B,  1904,  37. 
4329;  Eidmann,  C.  C.,  1899,  II.  1014.) 

Insol.  in  pyridine.  (Naumann,  B.  1904, 
37.  4601.) 

Thallic  iodide,  TlI3i 

Sol.  in  alcohol. 

Decomp.  slowly  in  the  air.  (Wells,  Z. 
anorg.  1894,  6.  313.) 

Sol.  in  ether. 

Thallothallic  iodide,  T13I4  =  5T1I,  T1I3. 
Sol.  in  H2O.    (Jorgensen,  J.  pr.  (2)  6*  82.) 

Thallium  nitride. 

Very  unstable.  (Franz  Fischer,  B.  1901, 
43.  1470.) 

Thallous  oxide,  T12O. 

Deliquescent.    Sol.  in  H2O. 
See  Thallous  hydroxide. 

Thallic  oxide,  T12O8. 

Insol.  in  H2O.  Not  attacked  by  cold 
H2SO4.  Sol.  in  hot  H2SO4.  Sol.  in  cold  HC1 
+Aq. 

Insol.  in  alkalies +Aq.      (Werther,  J.  pr 
91.  385.) 
Black  modification. 

Less  sol.  in  dil.  acids  than  the  brown 
modification.  Solution  is  accompanied  by 
a  slight  reduction  to  thallous  salt. 

More  sol.  in  10%  HC1  than  in  10%  H2SO4 
or  HNO3. 

More  sol.  in  cone,  than  in  dil.  acids.  (Rabe 
Z.  anorg.  1906,  48.  431.) 


Brown  modification. 

Easily  sol.  in  dil.  mineral  acids  on  warm- 
ng,  with  slight  reduction  to  thallous  salt. 

More  sol.  in  cone.  acid.    (Rabe.) 

Thallium  dioxide,  T1O2. 

Insol.  in  H2O.  (Piccini,  Gazz.  ch.  it.  17. 
450.) 

Thallic  oxide  ammonia,  T12O3,  6NH3. 

Decomp.  by  much  H2O.  Insol.  in  alcohol. 
(Carstanjen.) 

Thallic  oxyfluoride,  T1OF. 

Insol.  in  H2O.  Slowly  decomp.  by  boiling 
with  H2O. 

Sol.  in  mineral  acids.  Almost  insol.  in  HF. 
(Gewecke,  A.  1909,  366.  226.) 

Thallium  phosphide  (?). 
Ppt.     (Crookes.) 

Thallous  selenide,  Tl2Se. 

Insol.  in  H2O.  Scarcely  attacked  by  cold 
dil.  H2SO4+Aq,  but  dissolves  when  heated. 
(Carstanjen.) 

Thallothallic  selenide. 

Not  attacked  by  cold  cone,  or  boiling  dil. 
H2SO4+Aq.  Cone.  H2SO4  decomposes.  (Car- 
stanjen.) 

Thallous  sulphide,  T12S. 

Insol.  in  H2O,  (NH4)2S+Aq,  NH4OH+Aq 
KCN+Aq,  and  in  alkali  carbonates,  and 
hydrates  +Aq.  Difficultly  sol.  in  a  solution 
of  oxalic  acid  or  acetic  acid.  (Crookes.) 
Easily  sol.  in  HNO3,  and  H2SO4+Aq.  Diffi- 
cultly sol.  in  HCl+Aq.  (Willm.) 

SI.  sol.  in  H2O. 

0.21  X10-4  g.  is  dissolved  in  1  1.  sat.  solu- 
tion at  20°.  (Bottger,  Z.  phys.  Ch.  1903,  46. 
603.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Thallic  sulphide,  T12S3. 

Insol.  in  H2O.  Insol.  in  cold,  sol.  in  warm 
dil.  H2SO4+Aq  without  separation  of  S. 
Sol.  in  other  dilute  acids  with  separation  of  S. 
(Carstanjen.) 

Thallium  pentasulphide,  T12S6. 

Ppt.    (Hofmann,  B.  1903,  36.  3092.) 

Thallothallic  sulphide,  5T12S,  3T12S3. 

Very  slowly  decomp.  by  cold  dil.  £[2804+ 


T12S3.     (Carstanjen.) 
T12S,    2T12S3.      Decomp.    by    dil.    acids. 
(Schneider,  J.  pr.  (2)  10.  55.) 

Thallium  teUuride,  Tl2Te. 
(Fabre,  C.  R.  105.  673.) 


1060 


THIOANTIMONIC  ACID 


Thio- 

For  compounds  with  prefix  thio-,  see  also 
under  sulpho-. 

Thioantimonic  acid. 
See  Sulphantimonic  acid. 

Thioarsenic  acid. 
See  Sulpharsenic  acid. 

Thiomolybdic  acid. 
See  Sulphomolybdic  acid. 

Thionamic  acid,  NH3S02  =  NH2SO(OH). 

Very  deliquescent,  and  sol.  in  H2O. 

H2O  solution  decomp.  gradually.  (Rose, 
Pogg.  33.  275;  42.  425.) 

Ammonium   thionamate,    NH2SO(ONH4). 

Deliquescent.  Sol.  in  H2O;  easily  decomp. 
when  in  solution.  (Rose.) 

Very  sol.  in  alcohol  with  decomp.  SI.  sol. 
in  dry  ether.  (Divers  and  Ogawa,  C.  C.  1900, 
I.  1259.) 

Dtthionic  acid. 
See  Dithionic  acid. 

TVtthionic  acid. 
See  Trithionic  acid. 

Tetraihiomc  acid. 
See  Tetrathionic  acid. 

Penlathiomc  acid.  . 
See  Pentathionic  acid. 

Thionyl  bromide,  SOBr2. 

Unstable. . 

Decomp.  by  H2O.  (Besson,  C.  R.  1896, 
122.  322.) 

Thionyl  bromochloride,  SOClBr. 

Decomp.  slowly  in  the  cold,  rapidly  at  115°. 

Deccmp.  by  H2O.  (Besson  C.  R.  1896, 
122.  321.) 

Thionyl  chloride,  SOC12. 

Sol.  in  CHC13,  and  CeHe.  (Oddo,  Gazz.  ch 
it.  1899,  29.  (2)  318.) 

Thionyl  fluoride,  SOF2. 

Decomp.  by  H2O. 

Sol.  in  AsCl3,  CeH«,  ether  and  oil  of  turpen- 
tine, (Moissan,  C.  R.  1900,  130.  1439.) 

Thiophosphamic  acid,  H2PNH2O2S  (?). 

Known  only  in  its  salts.  (Gladstone  and 
Holmes,  Chem.  Soc.  (2)  3. 1.) 


Cadmium  thiophosphamate,  CdPNH202S. 

Sol.  in  dil.  acids.*  and  NH4OH+Aq.  (G. 
and  H.) 

Lead ,  PbPNH202S. 

Ppt.  Sol.  in  dil.  HNO3+Aq.  (Gladstone 
and  Holmes,  Chem.  Soc.  (2)  3.  1.) 

Thiophosphocfa'amic  acid,  H2PN2H4OS. 

Known  only  in  solution,  which  soon  de- 
composes. (G.  and  H.) 

Cadmium  thiophosphocfo'amate, 

Cd(PN2H4OS)2. 

Insol.  in  H2O;  sol.  in  dil.  acids,  and  NH4OH 
H-Aq.  (G.  and  H.) 

Cupric ,  Cu(PN2-H4OS)2. 

Insol.  in  H2O,  dil.  HC1,  or  NH4OH+Aq. 
Sol.  in  KCN+Aq.  (Gladstone  and  Holmes. 
Chem.  Soc.  (2)  3.  1.) 

Lead ,  Pb(PN2H4OS)2. 

Insol.  in  H2O.    Sol.  in  dil.  HNO3+Aq. 

Nickel ,  Ni(PN2H4OS)2. 

Sol.  in  dil.  acids,  and  NH4OH+Aq.  (Glad- 
stone and  Holmes,  Chem.  Soc.  (2)  3.  1.) 

Zinc  — ,  Zn(PN2H4OS)2. 

Ppt.  Sol.  in  dil.  acids,  and  NH4OH+Aq. 
(Gladstone  and  Holmes.) 

Thiophosphonitrile,  PSN. 

Not  decomp.  by  cold  H2O.  Slowly  decomp. 
by  boiling  H2O.  Easily  decomp.  by  boiling 
dil.  HC1.  (Stock,  B.  1906,  39.  1974.) 

Thiophosphoric  acid,"  H3PSO3=PS(OH)3. 
Known  only  in  its  salts. 

Ammonium   magnesium   thiophosphate, 

NH4MgPS03+9H20. 

SI.  sol.  in  cold  H2O.  (Kubierschky,  J.  pr. 
(2)  31. 100.) 

Barium  — ,  Ba3(PSO3)2. 

Insol.  in  H2O.    (Wurtz,  A.  ch.  (3)  20.  473.) 

Cobalt . 

Insol.  in  H2O,  but  partially  decomp.  when 
boiled  therewith.  (Wurtz.) 

Cupric . 

Insol.  in  H2O ;  very  easily  decomp.  (Wurtz.) 

Ferric  — . 

Insol.  in  H2O.    (Wurtz.) 

Magnesium ,  Mg3(PSO3)2+20H2O. 

SI.  sol.  in  cold  H2O.    (Kubierschky,  J.  pr. 


THIOPHOSPHORYL  CHLORIDE 


1061 


Nickel  thiophosphate. 

Insol.  in  H2O,  but  decomp.  when  boiled 
therewith.     (Wurtz.) 

Potassium  — ,  K3PSO8. 

Very  sol.  in  H2O.    Known  only  in  aqueous 
solution.     (Wurtz.) 

Sodium ,  Na3PSO3+12H2O. 

Easily  sol.  in  boiling  H2O.    Cryst.  out  on 
cooling.    (Wurtz,  A.  ch.  (3)  20.  472.) 

Insol.  in  alcohol. 

Strontium  — — . 

Insol.  in  H2O.    (Wurtz.) 

Dithiometaphosphoric  acid. 

Ammonium  cfo'thioraetaphosphate, 

NH4PS2O. 

Decomp.    by  H2O.     (Stock,  B.  1906,  39. 
1990.) 

Monothioorthophosphoiic  acid. 


woriothioor^ophosphate, 
O:P(SNH4)(OH)2. 
Sol.  in  H2O. 
Insol.  in  alcohol.    (Stock,  B.  1906,  39.  1990. 

Tnammonium  monothioortAophosphate, 

SNH4.PO.(ONH4)2. 
(Stock.) 

IH'thioortAophosphoric  acid. 

Ammonium  ^'thiophosphate,  (NH4)3PS2O2-{- 

2H20. 

81.  efflorescent.  Sol.  hi  H2O.  (Kubier- 
schky, J.  pr.  (2)  31.  93.) 

Ammonium  magnesium  — — •,  NH4MgPS202 

+6H20. 
81.  sol.  in  cold,  H2O.    (Kubierschky.) 

Barium ,  Ba3(PS2O2)2+8H2O. 

Precipitate.  (Kubierschky,  J.  pr.  (2)  31. 
103.) 

+  18H2O.  As  the  Zn'thio  compound. 
(Ephraim,  B.  1910,  43.  287.) 

Calcium . 

Very  easily  decomposed.     (Kubierschky.) 

Sodium ,  Na3PS2O2+llH2O. 

Very  sol.  in  H2O.  (Kubierschky,  J.  pr. 
(2)  31.  93.) 

Tn'thioortAophosphoric  acid. 

Ammonium  /n'thioor^Aophosphate, 

(NH4)3PS30+H20. 
(Stock,  B.  1906,  39.  1985.) 


Barium  /nthioor^ophosphate,  Ba3(PS8O)2+ 
20H20. 

Decomp.  by  H2O  and  dil.  acids. 

Sol.  in  cone.  HNO3  with  oxidation  of 
the  sulphur  to  H2SO4.  (Ephraim,  B.  1910, 


43 


e  sulp 

.  286. 


Magnesium ,  Mg8(PS30)2+20H20. 

Decomp.  by  H2O  and  dil.  acids.    (Ephraim. 

Thiophosphorous  acid. 

Ammonium  thiophosphite  (?),  (NH4)4P2S20| 

+3H20. 

Sol.  in  H2O.  (Lemoine,  C.  R.  98.  45.) 
+6H20. 

Sodium  thiophosphite  (?),  Na4P2S2O3+5H2O 

=  P2O3,  2Na2S+5H2O. 
Sol.  in  H2O.    (Lemoine.  C.  R,  98.  45.) 
Na6P2S2O4+4H2O  =  P203,  3Na2O,  2H2S+ 

2H2O.    Sol.inH2O.    (Lemoine,  I.e.) 

Thiophosphoryl  tfn'amide,  PS(NH2)3. 

Rapidly  decomp.  by  H2O.  Scarcely  sol. 
in  alcohol,  ether,  or  CS2.  (Chevrier,  C.  R.  66. 
748.) 

Metathiophosphoryl  bromide,  PS2Br. 

Decomp.  by  H2O.  Insol.  in  ether.  (Mich- 
aelis, A.  164.  9.) 

On'Aothiophosphoryl  bromide,  PSBr8. 

Slowly  decomp.  by  cold,  rapidly  by  hot  H2O 
but  volatile  with  only  partial  decomp.  with 
steam.  Easily  sol.  in  ether,  CS2,  PC18,  PBra. 
Decomp.  by  cold  alcohol.  Forms  hydrate 
PSBr3+H2O.  (Michaelis,  A.  164.  9.) 

Pi/rothiophosphoryl  bromide,  P2S8Br4. 

Decomp.  by  H2O  and  alcohol.  Sol.  hi  CSf 
and  ether.  (Michaelis.) 

Thiophosphoryl  phosphorus  bromide, 

PSBr3,  PBr3. 
Decomp.  by  H2O  into  PSBr3.    (Michaelis.) 

Thiophosphoryl  cfabromochloride,  PSClBr2. 

Decomp.  by  H2O  and  alkalies. 

Fumes  in  the  air.  (Besson,  C.  R.  1896, 
122.  1059.) 

Thiophosphoryl  bromoofo'chloride,  PSCl2Br. 

Decomp.  by  H2O  and  alkalies.  Reacts 
violently  with  HNO8.  (Besson,  C.  R.  1896, 
120.  1058.) 

Thiophosphoryl  chloride,  PSC18. 

Very  slowly  decomp.  by  H2O,  and  may 
be  distilled  with  steam  without  much  decomp. 
Decomp.  by  alcohol.  Miscible  with  CS2. 
(Baudrimont,  J.  pr.  87.  301.) 

Sol.  in  CC14  and  C6H6.  (Oddo,  Gazz.  ch. 
it.  1899,  29.  (2)  318.) 


1062 


THIOPHOSPHORYL  CHLORIDE 


Thiophosphoryl  pentachloride,  PS2C15  (?). 
Decomp.  by  H2O.  Sol.  in  alkalies  with 
residue  of  S.  Attacked  violently  by  HNO3, 
alcohol,  ether,  oil  of  turpentine.  Miscible 
with  CS2.  (Gladstone,  Chem.  Soc.  3.  5.) 

Thiophosphoryl  fluoride,  PSF3. 

Slowly  sol.  in  H2O  with  decomp.  SI.  sol. 
in  ether. 

Insol.  in  H2SO4,  CS^  or  benzene.  (Thorpe 
and  Rodger,  Chem.  Soc.  66.  306.) 

More  sol.  in  KOH  or  NaOH+Aq  than  in 
H20. 

Thiophosphoryl  iodide,  P2SI2. 

Very  sol.  in  CS2.  Unstable  when  heated. 
Fumes  in  the  air.  (Besson,  C.  R.  1896,  122. 
1201.) 

Thiosulphuric    (formerly    Hyposulphur- 

ous)  acid,  H2S3O3. 

Known  only  in  aqueous  solution,  which  is 
extremely  unstable,  and  decomposes  very 
quickly  after  its  formation.  The  time  before 
decomposition  is  exactly  proportional  to  the 
ratio,  of  the  weight  of  H2O  to  the  weight  of 
H2S2O3  present;  i.  e.,  if  one  solution  contains 
twice  as  much  H2O  for  a  given  amt.  of  H2S2p3 
as  a  second  solution,  the  first  solution  will 
decompose  in  twice  the  length  of  time.  The 
length  of  time  is  about  20  sees,  at  10°,  and 
2  sees,  at  50°  for  cone,  solutions,  to  120  sees, 
at  10°  and  12  sees,  at  50°  for  very  dilute  solu- 
tions. (See  Landolt  (B.  16.  2958)  for  further 
figures;  also  Winkelmann  (B.  18.  406). 

Thiosulphates. 

The  thiosulphates  of  the  alkalies  and  of 
Ca  and  Sr  are  easily  sol.  in  H2O;  Ba  and  Sr 
salts  are  si.  sol.  and  the  other  salts  insol.  The 
salts  of  the  metals  dissolve  in  alkali  thiosul- 
phates +  Aq.  All  are  insol.  in  alcohol. 

Double  Salts  of  Thiosulphuric  acid.  It  is 
impossible  to  determine  whether  substances 
of  this  class  are  true  chem .  individuals.  Many 
described  by  Svensson  and  others  are  doubt- 
less isomorphic  mixtures,  whose  comp.  de- 
pends on  the  temp,  and  cone,  of  the  solution 
in  which  pptd.  (Rosenheim,  Z.  anorg.  1900 
25.72.) 

Ammonium    thiosulphate,    (NH4)2S203. 

Very  deliquescent.    Very  sol.  in  H2O. 

Not  deliquescent.  (Fock  and  Kliiss,  B. 
1889,  22.  3099.) 

Crystallises  with  VsH^O.  (Rammelsberg, 
Pogg.  66.  298.)  Anhydrous.  (Arppe,  A.  96. 
113.) 

Insol.  in  alcohol.    (Arppe.) 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899. 
II.  1014.) 

Difficultly  sol.  in  acetone.  (Naumann,  B. 
1904,  37.  4328.) 


Ammonium  cadmium  thiosulphate, 

3(NH4)2S2O3,  CdS2O3+3H2O. 
Can  be  recryst.  from  warm  H2O. 
and  Kliiss,  B.  23.  1758.) 
+H2O.    (F.  and  K.) 

(NH4)2S203,  CdS2O3.    (F.  and  K.) 


(Fock 


Ammonium  cuprous  thiosulphate, 

(NH4)2S2O3,  Cu2S2O3+2H2O. 

Less  sol.  in  H2O  than  2(NH4)2S2O3, 
Cu2S2O3  +  l^H2O.  (Rosenheim  and  Stein- 
hauser, Z.  anorg.  1900,  26.  91.) 

2(NH4)2S203,  Cu2S203+l^H20.  Very 
sol.  in  H2O.  Insol.  in  alcohol.  (Rosenheim 
and  Steinhauser.) 

Ammonium  cuprous  thiosulphate  cuprous 
iodide,  7(NH4)2S203,  Cu2S2O3,  8CuI+ 
4H2O. 

Insol.  in  H2O.    (Brun,  C.  R.  1892, 114.  668.) 
Could  not  be  obtained.     (Rosenheim  and 
Steinhauser,  Z.  anorg.  1900,  26.  107.) 

Ammonium    cuprous    sodium    thiosulphate 
ammonia,    3Cu2S2O3,     4Na2S2O3, 
(NH4)2S203,  6NH3. 

Ppt.    When  dry  is  fairly  stable  in  the  air. 
Partially  decomp.  by  H2O. 
Sol.  in  dil.  H2SO4  or  acetic  acid.     (Shinn, 
J.  Am.  Chem.  Soc.  1904,  26.  948.) 

Ammonium  lead  thiosulphate,  2(NH4)2S2O8, 

PbS2O3+3H2O. 

Easily  and  completely  sol.  in  cold  H2O,  but 
deposits  PbS2O3  by  standing  or  warming. 
(Rammelsberg,  Pogg.  66.  312.) 

Ammonium  magnesium  thiosulphate, 

rNH4)2Mg(S2O3)2+6H2O. 

Very  deliquescent,  and  sol.  in  H2O.  (Kess- 
ler,  Pogg.  74.  283.) 

Not  deliquescent.  (Fock  and  Kliiss,  B. 
23.  540.) 

Ammonium  mercuric  thiosulphate, 

4(NH4)2S203,  HgS203+2H20. 
Sol.  in  H2O,  from  which  it  is  precipitated 
by  alcohol.    Extremely  easily  decomp.    (Ram- 
melsberg, Pogg.  56.  318.) 


Ammonium  potassium  thiosulphate, 

NH4KS2O3. 
Sol.  in  H2O.    (Fock  and  Kliiss,  B. 


I.  536.) 


Ammonium  silver  thiosulphate,  2(NH4)2S2O3, 
Ag2S2O3+zH2O. 

Easily  sol.  in  H2O.  Somewhat  sol.  in  alco- 
hol. (Herschel,  Edinb.  Phil.  J.  1.  398.) 

(NH4)2S2O3,  Ag2S2O3+xH2O.  Nearly  in- 
sol. in  H2O;  sol.  in  NH4OH+Aq,  from  which 
it  is  repptd.  by  an  acid.  (Herschel.) 


THIOSULPHATE,  BISMUTH  POTASSIUM 


1063 


Ammonium  zinc  thiosulphate, 
3,  ZnS2O3+H2O. 


Very  sol.  in  H2O.  (Rosenheim  and  David- 
sohn,  Z.  anorg.  1904,  41.  238.) 

Ammonium  thiosulphate  ammonium  cuprous 
bromide,  CuBr,  NHiBr,  4(NJI4)2S2O3. 

Sol.  in  H2O.  (Rosenheim,  Z.  anorg.  1900, 
26.  107.) 

The  double  salts  of  ammonium  thiosul- 
phate with  silver  and  copper  haloids  are  true 
chemical  compounds  and  may  be  recryst. 
from  H2O  without  decomp.  (Rosenheim,  Z. 
anorg.  1900,  25.  100.) 

Ammonium  thiosulphate   ammonium   silver 
bromide,   AgBr,    NH4Br,   4(NH4)2S2O3. 
Sol.  in  H2O.    (Rosenheim.) 

Ammonium  thiosulphate  ammonium  cuprous 

chloride,  CuCl,  NH4C1,  4(NH4)2S2O3. 
Sol.  in  H2O  and  in  NH4OH+Aq.    (Rosen- 
heim.) 

Ammonium  thiosulphate   ammonium   silver 

chloride,  AgCl,  NH4C1,  4(NH4)2S2O3. 
Sol.  in  cold  H2O  and  NH4OH+Aq. 

Decomp.  by  boiling  with  H2O  and  by  dil. 
acids.  (Rosenheim.) 

Ammonium  thiosulphate  ammonium  cuprous 
cyanide. 

Composition  not  constant.     (Rosenheim.) 

Ammonium  thiosulphate  ammonium  silver 
cyanide. 

Composition  not  constant.     (Rosenheim.) 

Ammonium  thiosulphate  ammonium  cuprous 

iodide,  Cul,  NHJ,  4(NH4)2S203. 
Sol.  in  H2O.    (Rosenheim.) 

Ammonium  thiosulphate  ammonium  cuprous 

iodide,  4(NH4)2S2O3,  NHJ,  Cul. 
Very  sol.  in  H2O.     Decomp.  by  boiling. 
(Brun,  C.  R.  1892,  114.  668.) 

Ammonium   thiosulphate   ammonium   silver 

iodide,  Agl,  NH4I,  4(NH4)2S2O3. 
Sol.  in  H2O.    (Rosenheim.) 

Ammonium  thiosulphate  ammonium  cuprous 
sulphocyanide,  CuSCN,  NH4SCN, 

4(NH4)2S203. 
Sol.  in  H2O.    (Rosenheim.) 

Ammonium  thiosulphate  ammonium  silver 
sulphocyanide,  AgSCN,  NH4SCN, 

4(NH4)2S203. 
Sol.  in  H2O.    (Rosenheim.) 


Ammonium  thiosulphate  cuprous  iodide, 

(NH4)2S203,  2CuI+H20. 

Insol.  in  H2O.  (Brun,  C.  R.  1892,  114. 
668.) 

Could  not  be  obtained.  (Rosenheim  and 
Steinhauser.) 

Barium  thiosulphate,  BaSa03+H2O. 

SI.  sol.  in  H20.    (Rose,  Pogg.  21.  437.) 

Insol.  in  alcohol. 

1  pt.  cannot  be  dissolved  in  2000  pts.  H20. 
Sol.  in  dil.  HCl+Aq  without  decomposition. 
(Herschel,  1819.) 

Pptd.  from  BaS2O3+Aq  by  dil.  alcohol. 
(Sobrero  and  Selmi,  A.  ch.  (3)  28.  211.) 

Insol.  hi  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Barium  bismuth  thiosulphate,  Ba3[Bi(S20»)l]j. 
Sol.  in  H2O  with  decomp.      (Hauser,   Z. 
anorg.  1903,  36.  9.) 

Barium  cadmium  thiosulphate,  2BaS2O8, 

CdS203+8H20. 

SI.  sol.  in  H2O.     (Fock  and  Kliiss,  B.  23. 
1761.) 
3BaS2O3,  CdS2O3+8H2O.    SI.  sol.  in  H2O. 

Barium  cuprous  thiosulphate. 

Easily  sol.  in  hot,  difficultly  sol.  in  cold 
H2O.  (Cohen,  Chem.  Soc.  61.  38.) 

2BaS2O3,  Cu2S2O3-t-7H2O.  Nearly  insol. 
in  H2O.  (Vortmann,  M.  9.  165.) 

Barium  gold  thiosulphate. 

SI.  sol.  in  H2O.  Insol.  in  alcohol  (Fordos 
and  Gelis.) 

Barium  lead  thiosulphate. 

Difficultly  sol.  in  H2O.  (Rammelsberg, 
Pogg.  66.  313.) 

Barium  thiosulphate  chloride,  BaS2O8, 

BaCl2+2H2O. 
Sol.  in  H2O.    (Fock  and  Kliiss,  B.  23.  3001.) 

Bismuth  caesium  thiosulphate,  Cs3Bi(S2O8)8. 

Sol.  in  H2O. 

Insol.  in  alcohol.  (Hauser,  Z.  anorg.  1903, 
36.  8.) 


Bismuth  potassium  thiosulphate, 


Solubility  in  H20. 

100  cc.  of  the  sat.  solution  contain  3.5  g. 
at  2°;  7.0  g.  at  18°.  At  18°  the  solution 
decomposes. 

More  sol.  in  Na2S2O3+Aq  than  in  pure 

TT  r\ 

Insol.  in  alcohol.    (Hauser,  Z.  anorg.  1903, 

*+H2O  Sol.  in  H2O.  Insol.  in  alcohol. 
(Carnot,  C.  R.  83.  390.) 


1064 


THIOSULPHATE,  BISMUTH  RUBIDIUM 


Bismuth  rubidium  thiosulphate, 

Rb3Bi(S203)3+^H20. 

Sol.  in  H2O. 

Insol.  in  acid  alcohol.  (Hauser.  Z.  anorg. 
1903,  36.  7.) 

+H2O.  Sol.  in  H2O.  (Hauser,  Z.  anorg. 
1903,  36.  8.) 

Bismuth  sodium  thiosulphate, 

Very  sol.  in  H2O,  and  also  in  alcohol. 
(Carnot,  C.  R.  83.  338.) 

Na3Bi(S2O3)3.  Decomp.  by  H2O.  Easily 
sol.  in  50%  alcohol.  (Hauser,  Z.  anorg.  1903, 
35.  3.) 

Cadmium  thiosulphate,  CdS2O3+2H2O. 

Sol.  in  H2O.  Insol.  in  alcohol.  (Vortmann 
and  Padberg,  B.  22.  2638.) 

Cadmium  potassium  thiosulphate,  3CdS203, 
5K2S2O3. 

Cannot  be  recryst.  without  decomp.  (Fock 
and  Kluss,  B.  23.  1753.) 

CdS2O3,  3K2S2O3+2H2O.  Can  be  crystal- 
lised from  H2O  without  decomp.  (F.  and  K.) 

Cadmium  sodium  thiosulphate,  CdS2O3, 
3Na2S2O3+16H2O. 

Not  deliquescent.  Sol.  in  H2O.  (Jochum, 
C.  C.  1885,  642.) 

+9H2O.  (Vortmann  and  Padberg,  B.  22. 
2639.) 

+3H2O.  Deliquescent.  (Fock  and  Kluss, 
B.  23.  1157.) 

2CdS2O3,  Na2S2O3+7H2O.    (V.  and  P.) 

3CdS2O3,  Na2S2O3+9H2O.    (V.  and  P.) 

Cadmium   strontium   thiosulphate.    CdS2O3) 

3SrS2O3+10H2O. 
(Fock  and  Kluss,  B.  23.  1763.) 

Caesium'  thiosulphate,  Cs2S2O8. 

Easily  sol.  in  H2O.  (Chabrie",  C.  R.  1901, 
133.  297.) 

+2H2O.  Very  hydroscopic.  (J.  Meyer, 
B.  1907,  40.  1360.) 


Caesium  cuprous  thiosulphate,  Cs2S2O3, 

Easily    sol.    in    H2O    with    decomp. 
Meyer,  B.  1907,  40.  1361.) 


(J. 


Caesium  lead  thiosulphate,  Cs2S2O3,  PbS203 
+2H20. 


Not  hydroscopic. 
2Cs2S2O3,    PbS2O3+3H2O. 
(J.  Meyer.) 


Hydroscopic. 


Caesium  magnesium  thiosulphate,  Cs2S2O3, 

MgS208+6H20. 
Easily  sol.  in  H2O.    (Meyer.) 


Caesium  silver  thiosulphate,  2Cs2S2O3, 

Ag2S203+3H20. 
Not  hydroscopic. 
Decomp.  by  hot  H2O.     (J.  Meyer.) 

Calcium  thiosulphate,  CaS2O3+6H2O. 

Sol.  in  1  pt.  H2O  at  3°. 

Aqueous 'solution  saturated  at  10°  has  sp. 
gr.  1.300.  Solution  with  sp.  gr.  1.11437  at 
15.5°  contains  0.2081  of  its  weight  in  CaS2O3. 

Decomp.  on  heating.  Insol.  in  alcohol 
(sp.  gr.  0.8234).  (Herschel,  A.  ch.  14.  355.) 

100  g.  sat.  solution  contains  29.4  g.  CaS203 
at  9°,  and  34.7  g.  CaS2O3  at  25°.  (Kremann 
and  Rodemund,  M.  1914,  35.  1065.) 

Solubility  of  CaS2O3+Na2SO3  in  H2O. 


t° 

o/ 

NfttfiOi 

% 
CaS2Os 

Solid  phase 

9 

0 
11.04 
25.21 
31.01 

29.4 
22.64 
15.84 
7.70 

CaS2O3,  6H2O 
(e 

"     +Na2S2O3,  5H2O 
Na2S203,  5H20 

25 

0 

9.24 
15.67 
18.34 
28.24 
30.19 
31.24 
35.04 

34.7 
29.69 
21.41 
25.18 
21.14 
20.33 
18.43 
11.61 

CaS203,  6H2O 
(i 

u 

(C 

(( 

"     +Na2S203,  5H2O 

Na2S2O3,  5H2O 
a 

(Kremann  and  Rodemund,  M.  1914,  35.  1065.) 

Calcium  lead  thiosulphate,  2CaS2O3,  PbS2O3 

+4H20. 
Decomp.  by  H2O.    (Rammelsberg.) 

Calcium    potassium    thiosulphate,    CaS2O8, 

3K2S203+5H20. 
Sol.  in  H2O.    (Fock  and  Kluss,  B.  24.  3016.) 

Calcium  silver  thiosulphate,  2CaS2O3,  Ag2S203 


Easily  sol.  in  H2O;  less  sol.  in  alcohol. 

CaS2O3,  Ag2S2O3+.rH2O.  SI.  sol.  in  H2O, 
abundantly  in  NH4OH+Aq.  (Herschel, 
1819.) 

Calcium  sodium  thiosulphate  nitrate,      . 
CaNa3(S2O3)2NO3+llH2O. 

(Kremann  and  Rothemund,  M.  1914,  35. 
1065.) 

Cobaltous  thiosulphate,  CoS2O8+6H2O. 
Sol.  in  H2O.    (Rammelsberg.) 

Cobaltous    sodium    thiosulphate,    2CoS208, 

5Na2S203+25H20. 

Efflorescent.    Sol.  in  H2O.     (Jochum.) 
Could  not  be  obtained  by  Vortmann  and 

Padberg. 


THIOSULPHATE,  CUPRIC  SULPHIDE,  CUPRIC  SODIUM 


1065 


CoS2O3,  3Na2S2O3  +  15H2O.  Sol.  in  H2O. 
(Vortmann  and  Padberg,  B.  22.  2641.) 

Cuprous  thiosulphate,  Cu2O,  3S2O2+2H2O  = 

Cu2H4(S203)2. 

SI.  sol.  in  H2O.  Abundantly  sol.  in  Na2S2O3 
+  Aq,  NH4C1  +  Aq,  NH4OH  +  Aq,  or 
(NH4)2CO3+Aq.  Sol.  in  HC1  or  HNO3+Aq. 
(v.  Hauer,  W.  A.  B.  13.  443.) 

Cuprous  hydrazine  thiosulphate, 

Cu2S203,  (N2H4)2H2S20 


Insol.  in  H2O;  sol.  in  NH4OH+Aq  and  in 
dU.  acids.  (Ferratini,  C.  C.  1912,  I.  1281.) 

Cupric  lead  thiosulphate,  Pb(CuS2O3)2 

+3H20.  (?) 

Very  sol.  in  H2O  and  quickly  decomp. 
(Girard,  C.  C.  1904,  I.  253.) 

Cuprous  mercurous  thiosulphate,  5Cu2S2O3. 

3Hg2S2O3. 

Insol.  or  si.  sol.  in  cold,  decomp.  by  boiling 
H2O.  HNO3+Aq  dissolves  out  Cu.  (Ram- 
melsberg,  Pogg.  66.  319.) 

Cuprous  potassium  thiosulphate,  Cu2S2O3, 
K2S2O3+2H2O. 

SI.  sol.  in  H2O;  decomp.  on  heating  with 
pptn.  of  CuS.  Easily  sol.  in  K2S2O3+Aq. 
(Rammelsberg,  Pogg.  56.  321.) 

Cu2S2O3,  2K2S2O3.  Very  sol.  in  cold  H2O; 
insol.  in  K2S2O3+Aq.  (Cohen,  Chem.  Soc. 
61.  39.) 

+3H2O.  Scarcely  sol.  in  cold,  sol.  with  si. 
decomp.  in  hot  H2O.  Sol.  in  HCl+Aq  with 
evolution  of  SO2. 

Cu2S2O3,  3K2S2O3+3H2O.  More  sol.  in 
H2O  than  Cu2S2O3,  K2S2O3+2H2O.  Solution 
is  not  decomp.  by  boiling.  Sol.  in  excess  of 
NH4OH+Aq.  (Rammelsberg.) 

Cuprous    rubidium    thiosulphate,    Rb2S2O3, 

Cu2S203+2H20. 

Ppt.    (J.  Meyer,  B.  1907,  40.  1357.) 
2Rb2S2O3,     Cu2S203+2H2O.       Ppt.       (J. 


Meyer.) 

3Rb2S2O3,     Cu2S2O3+2H2O. 
Meyer.) 


Ppt.       (J. 


Cuprous    saver    sodium    thiosulphate    am- 
monia,   Cu2S2O8,    2Ag2S2O3,    5Na2S2O3, 
6NH3. 
Ppt.    Becomes  dark  when  exposed  to  light. 

Decomp.    by    H2O.      Sol.    in    NH4OH+Aq. 

(Shinn,  J.  Am.  Chem.  Soc.   1904,  26.  949.) 

Cuprous  sodium  thiosulphate,  2Cu2S2O3, 
7Na2S208+2H20. 

Ppt.  from  aqueous  solution  by  alcohol. 
(Jochum,  C.  C.  1886.  642.) 

+  12H2O.  Sol.  in  very  dil.  HCl+Aq. 
(Jochum-.) 


Cu2S2O3,  3Na2S2O3+2H2O.  Sol.  in  H2O; 
insol.  in  alcohol.  (Rammelsberg.) 

+6H2O.    (Jochum.) 

3Cu2S2O3,  2Na2S2O3+8H2O.  Decomp.  by 
H.2O.  (Vortmann.) 

+5H2O.  (Lenz,  A.  40.  99.)  Formula  ac- 
cording to  Jochum  is — 

5Cu2S2O3,  4Na2S2O3+8H2O.  Insol.  in  H2O 
or  alcohol.  Sol.  in  HCl+Aq  without  evolu- 
tion of  SO2,  also  in  dil.  H2SO4  or  HNO3+Aq. 
Sol.  in  NH4OH+Aq.  (Jochum.) 

+6H2O.    As  above.    (Jochum.) 

Cu2S2O3,  Na2S2O3+H2O.  Insol.  in  H2O; 
sol.  in  Na2S2O3+Aq.  (Russell,  Ch.  Ztg.  9. 
233.) 

+2H2O.    Insol.  in  H2O  and  alcohol. 

Decomp.  by  dil.  acids.  (Rosenheim  and 
Steinhauser,  Z.  anorg.  1900,  25.  84.) 

+2^H2O.  Sol.  in  H2O.  Pptd.  by  alcohol. 
(Bhaduri,  Z.  anorg.  1898,  17.  1.) 

+3H2O.  Decomp.  by  H2O.  (Vortmann, 
M.  1888,  9.  168.) 

3Cu2S2O3,  2Na2S2O3.  (Gerard,  C.  C.  1904, 
I.  253.) 

+5H2O.     Sol.  in  352  pts.  H2O.     (Russell, 
Ch.  Z.  1885,  9.  223.) 
100  cc.  5%      Na2S203+Aq  dissolve  12.28  g. 

"  "  7.5%         "  "          17.46g. 

"  "10%  "  "          22.54g. 

(Russell,  Ch.  Z.  1885,  9.  223.) 

4Cu2S2O3,  3Na2S2O3+6H2O.  Insol.  in  H2O 
and  alcohol. 

Decomp.  by  dil.  acids.  (Rosenheim  and 
Steinhauser,  7.  anorg.  1900,  26.  84.) 

+9H2O.  Sol.  in  H2O.  Pptd.  by  alcohol. 
(Bhaduri,  Z.  anorg.  1898,  17.  1.) 

7Cu2S2O3,  5Na2S2O3  +  16H2O.  Decomp. 
by  H2O  and  by  alcohol.  (Bhaduri,  Z.  anorg. 
1898,  17.  1.) 

It  is  impossible  to  determine  whether  any 
of  these  compds.  are  complex  or  double  salts. 
As  a  class  they  are  not  easily  sol.  and  decomp. 
in  solution.  They  may  therefore  be  mixtures 
whose  comp.  depended  upon  the  temp,  and 
cone,  of  the  solution  in  which  they  were  pptd. 
(Rosenheim,  Z.  anorg.  1900,  26.  81.) 

Cuprocupric  sodium  thiosulphate  ammonia, 

Cu2S2O3,  CuS2O8,  2Na2S2O3,  4NHS. 
Insol.  in,  but  decomp.  by  hot  H20.     Sol. 
in  HC2H3O2+Aq.     Sol.  in~NH4OH+Aq  or 
Na2S2O3+Aq.      (Schutte,   C.   R.  42.    1267.) 

Cuprous  sodium  thiosulphate  cuprous  chlor- 
ide, Cu2S2O8,  2Na2S2O3,  2CuCl. 
(Rosenheim    and    Steinhauser,    Z.    anorg. 
1900,  26.  86.) 

Cupric  sodium  thiosulphate  cupric  sulphide, 

Cu2S2O3,  Na2S2O3,  CuS+4H2O. 
;     SI.  sol.  in  H2O;  easily  sol.  in  Na2S2O3+Aq, 
and  NH4OH+Aq;  insol.  in  alcohol.     (Lenz, 
A.  40.  99.) 

Cu2S2O3,  Na2P2O3,  2CuS.  Sol.  in  H2O  or 
dil.  HCl+Aq.  (Kessel,  B.  11.  1585.) 


1066 


THIOSULPHATE  SODIUM  CHLORIDE,  CUPROUS  SODIUM 


Cuprous  sodium  thiosulphate  sodium  chlor- 
ide, 3Cu2S2O3,  2Na2S2O3,  4NaCl+8H2O 

Sol.  in  Na2S2O3+Aq.  (Siewert,  Zeit.  ges 
Naturwiss.  26.  486.) 

Ppt.    (Bhaduri,  Z.  anorg.  1898,  17.  3.) 

Cupric  thiosulphate  ammonia,  CuS2O3, 

4NH3. 

100  pts.  H2O  dissolve  21.79  pts.  at  25° 
(Pudschies,  Dissert.) 

Cuprocupric  thiosulphate  ammonium  chlor- 
ide, Cu2O,  CuO,  3S2O2,  2NH4C1. 
Sol.  in  HNO3+Aq  with  separation  of  S. 
(v.  Hauer,  W.  A.  B.  13.  447.) 

Glucinum  thiosulphate,  G1S2O3+11H2O. 
(Faktor,  C.  C.  1901,  II.  878.) 

Gold  (aurous)   hydrogen   thiosulphate, 

Au2S203,  3H2S2O3. 

Known  only  in  solution.  (Fordos  and  Gelis, 
A.  ch.  (3)  13.  394.) 

Gold  (aurous)  sodium  thiosulphate,  Au2S203, 
3Na2S203+4H20. 

Sol.  in  H2O;  solution  decomp.  on  heating. 
Insol.  in  absolute,  si.  sol.  in  dil.  alcohol. 
(Fordos  and  Gelis.) 

Au2S2O3,  6Na2S2O3+10H2O.  Very  sol. 
in  H2O,  but  decomp.  by  boiling.  (Jochum,  C. 
C.  1885.  642.) 

Iron  (ferrous)  thiosulphate,  FeS2O3+5H2O. 

Deliquescent.  Very  sol.  in  H2O  or  alcohol. 
(Koene,-  Pogg.  63.  241.) 

Iron  (ferrous)  sodium  thiosulphate,  FeS2O3, 

3Na2S2O3+8H2O. 

Very  sol.  in  H2O,  and  easily  decomp. 
(Vortmann  and  Padberg,  B.  22.  2641.) 

Lead  thiosulphate,  PbS2O3. 

k  Sol.  in  3266  pts.  H2O.    Sol.  in  alkali  thio- 

sulphates   +Aq.     (Rammelsberg,   Pogg.  66. 

308.) 

Lead  lithium  thiosulphate,  PbS203,   Li2S2O3. 

Very  hydroscopic. 

Decomp.  by  H2O  with  separation  of  PbS. 
(J.  Meyer,  B.  1907,  40.  1355.) 

Lead   potassium   thiosulphate,   PbS2O3, 

3K2S203+2H20. 

Sol.  in  H2O  with  partial  separation  of 
PbS2O3.  Sol.  in  K2S2O3+Aq.  (Rammels- 
berg, Pogg.  56.  310.) 

Lead  rubidium  thiosulphate,  2Rb2S2O3, 
PbS203+2H20. 

Difficultly  sol.  in  cold  H2O. 

Decomp.  by  H2O.  (J.  Meyer,  B.  1907, 
40.  1358.) 


Lead  sodium  thiosulphate,  PbS2O3,  2Na2S2O8. 

SI.  sol.  in  H2O.  Very  easily  sol.  in  NaC2H3O2 
and  Na2S2O3+Aq.  (Lenz,  A.  40.  98.) 

Insol.  in  alcohol. 

2PbS2O3,  5Na2S2O3+60H2O.  Easily  de- 
comp. (Jochum,  C.  C.  1885.  642.) 

PbS2O3,  3Na2S2O3  +  12H2O.  Decomp.  in 
boiling  aqueous  solution.  (Vortmann  and 
Padberg,  B.  22.  2637.) 

Lead  strontium  thiosulphate. 

Sol.  in  H2O.  Precipitated  as  a  syrup  by 
alcohol.  (Rammelsberg.)  ;, 

Lithium  thiosulphate,  Li2S2O3+3H2O. 

Very  deliquescent,  and  sol.  in  H2O  and 
absolute  alcohol.  (Fock  and  Kluss,  B.  22. 
3099.) 

Lithium  silver  thiosulphate,  Li2S203,  Ag2S2O8 
+H2O. 

Hygroscopic. 

Decomp.  by  boiling  H2O  and  by  acids. 
(Meyer  and  Eggeling,  B.  1907,  40.  1355.) 

Magnesium  thiosulphate,  MgS2O3+6H2O. 

Very  easily  sol.  in  H2O.  Precipitated  from 
cone,  solution  by  alcohol.  (Rammelsberg, 
Pogg.  56.  303.) 

Magnesium  potassium  thiosulphate, 

MgK2(S203)2+6H20. 

Deliquescent,  and  sol.  in  H2O.  Less  sol. 
than  K2S2O3.  (Rammelsberg,  Pogg.  56.  304.) 

Not  deliquescent.  (Fock  and  Kluss,  B. 
23.  539.) 

Magnesium  rubidium  thiosulphate,  MgS2O8, 

Rb2S203+6H20. 
Easily  sol.  in  H2O.-    (Meyer.  B.  1907,  40. 

1358.) 

Manganous  thiosulphate,  MnS2O3. 

Sol.  in  H2O,  from  which  it  is  pptd.  by 
alcohol.  (Rammelsberg,  Pogg.  56.  305.) 

+5H2O.  Decomp.  very  easily.  (Vort- 
mann and  Padberg,  B.  322.  2641.) 

Manganous   sodium   thiosulphate,    MnS2O8, 

2Na2S203+16H2O. 

Sol.  in  H2O.  Insol.  or  but  si.  sol.  in  alcohol. 
(Jochum,  C.  C.  1885.  642.) 

Mercuric  potassium  thiosulphate,  3HgS2O8, 
5K2S203. 

Sol.  in  10  pts.  H2O  at  15°,  and  Y^  pt.  at 
100°.  Aqueous  solution  decomp.  on  stand- 
ing or  heating. 

Insol.  in  alcohlol.  (Kirchhoff,  Scher.  J. 
2.  30.) 

HgS2O3.  3K2S2O3+3H2O.  (Fock  and 
Kluss,  B.  24.  1353.) 

HgS2Q3,  5K2S203+H20.     (F.  and  K.) 


THIOSULPHATE,  SILVER  SODIUM 


1067 


Nickel  thiosulphate,  NiS2O3+6H2O. 

Permanent.    Sol.  in  H2O.     (Rammelsberg, 
Pogg.  66.  306.) 

Nickel    sodium    thiosulphate,    2NiS2O3, 

5Na2S2O3-f25H2O. 
Efflorescent.    Sol.  in  H2O.     (Jochum.) 

Nickel  thiosulphate  ammonia,  NiS2O8,  4NH3 
+6H20. 


Decomp.    on   air.      Sol.    in   NH4OH+Aq. 
'   306.) 

(Ephraim,  B.  1913, 

(Vortmann    and 


(Rammelsberg,  Pogg.  66.  306.) 
NiS2O3,  5NH3+H2O. 


46.  3108.) 

NiS2O3,    6NH3+3H2O. 
Padberg,  B.  22.  2641.) 

Platinous  sodium  thiosulphate. 
See  Platothiosulphate,  sodium. 

Potassium     thiosulphate,     K2S2O3+V3,     1, 

12/3H2O,  and  2H2O. 

Very  deliquescent.  Very  sol.  in  H2O  with 
absorption  of  heat.  Solution  is  stable  on  the 
air.  Insol.  in  alcohol. 

100  pts.  H2O  dissolve  pts.  K2S2O3  at  t°. 


t° 

Pts. 
K2S203 

Solid  phase 

0 

96.1 

K2S2O3.2H2O 

17 

150.5 

3K2S2O3.5H2O 

20 

155.4 

" 

25 

165.0 

" 

30 

175.7 

" 

35 

202.4 

3K2S2O3.5H2O+K2S2O3.H2O 

40 

204.7 

K2S2O3.H2O 

45 

208.7 

u 

50 

215.2 

a 

55 

227.7 

u 

60 

238.3 

n 

56.1 

234.5 

K2S2O3.H2O+3K2S2O3.H2O 

65 

245.8 

3K2S203.H20 

70 

255.2 

a 

75 

268.0 

it 

78.3 

292.0 

3K2S2O3.H2O+K2S2O3 

80 

293.1 

K2S203 

85 

298.5 

[( 

90 

312.0 

(i 

(Inohiko  lo,  Mem.  Coll.  Sc.  Kioto,  1911,  3. 

212.) 

Sol.  in  dil.  HC2H3O2+Aq  without  decomp. 
(Mathieu-Plessy,  C.  R.  101.  59.) 

Insol.  in  ethyl  acetate.  (Casaseca,  C.  R. 
30.  821.) 

Potassium  silver  thiosulphate,  2K2S2O3, 
Ag2S203. 

Sol.  inH2O.    (Cohen.) 

K2S2O3,  Ag2S2O3.  SI.  sol.  in  H2O.  (Her- 
schel.) 

3K2S2O3,  Ag2S2O3+2H2O.  Rather  si.  sol. 
in  H2O.  (Rosenheim  and  Steinhauser,  Z. 
anorg.  1900,  26.  76.) 

SI.  sol.  in  H2O.     (Rosenheim.) 


Potassium  silver  thiosulphate  ammonia, 
KAgS2O3,  2NH3. 

Very  si.  sol.  in  H2O.  Easily  sol.  in  hot 
NH4OH+Aq.  (Schwicker,  B.  22.  1735.) 

5K2S2O3,  3Ag2S2O3,  NH3.  Difficultly  sol. 
in  H2O  with  decomp. 

Sol.  in  hot  NH4OH+Aq  with  partial  de- 
comp. (J.  Meyer,  B.  1907,  40.  1359.) 

Potassium   sodium   thiosulphate. 

(a)  KNaS2O3+2H2O.  Very  sol.  in  H2O. 
100  pts.  H2O  dissolve  213.7  pts.  salt  at  15°. 
(Schwicker,  B.  22.  1733.) 

(6)  NaKS2O3+2H2O.  100  pts.  H2O  dis- 
solve 205.3  pts.  salt  at  15°.  (Schwicker.) 

Potassium   strontium   thiosulphate,   K2S2O3, 

SrS2O3+5H2O. 
Sol.  in  H2O.    (Fock  and  Kliiss,  B.  24.  3017.) 

Potassium  zinc  thiosulphate,  K2S2O3, 

ZnS2O3+H2O. 

Very  sol.  in  H2O.  (Rosenheim  and  David- 
sohn,  Z.  anorg.  1904,  41.  238.) 

Potassium  thiosulphate  sodium  chloride, 

K2S203,  NaCl. 
Sol.  in  H2O.     (Pape,  Pogg.  139.  238.) 

Rubidium  thiosulphate,  Rb2S2O3+2H2O. 
••  Very  hydroscopic;  easily  sol.  in  H2O.     (J. 
Meyer,  B.  1907,  40.  1356.) 

Rubidium  silver  thiosulphate,  2Rb2S203, 

Ag2S203+2H20. 

Ppt.  Not  hydroscopic.  Difficultly  sol.  in 
cold  H2O.  Decomp.  by  warm  H2O.  (J. 
Meyer.) 

Rubidium  silver  thiosulphate  ammonia, 
Rb2$2O3,  Ag2S2O3,  NH3. 

Ppt.     (J.  Meyer.) 

3Rb2S2O3,  4Ag2S2O3,  NH3.  Ppt.  Decomp. 
in  the  air.  (J.  Meyer.) 

Samarium  thiosulphate. 

(Cleve.) 

Scandium  thiosulphate,  basic,  Sc(OH)S2O3. 
Ppt.     (R..  J.  Meyer,  Z.  anorg.  1914,  86. 

282.) 

Silver  thiosulphate,  Ag2S2O8. 

SI.  sol.  in  H2O.  Sol.  in  NH4OH  or  alkali 
thiosulphates-{-Aq.  (Herschel,  Edinb.  Phil. 
J.  1.  26.) 

Silver  sodium  thiosulphate,    Ag2S2O«, 
Na2S2O3+H2O. 

SI.  sol.  in  H2O.  Easily  sol.  in  NH4OH  + 
Aq,  also  in  Na2S2O3+Aq  to  form— 

Ag2S2O3,  2Na2S2O3+2H2O.  Easily  sol.  in 
H2O  or  NH4OH+Aq;  somwehat  sol.  in*al- 


1068         THIOSULPHATE  ACETYLIDE  ACETYLENE,  SILVER  SODIUM 


cohol,  especially  if  warm  or  dilute.     (Lenz, 
A.  40.  94.) 

Ag2S2O3,  6Na2S2O3+21H2O.  Sol.  in  H2O. 
(Jochum,  C.  C.  1885.  642.) 

SUver  sodium  thiosulphate  acetylide  acety- 
lene, 2Na2S2O3,  7Ag2S2O3,  18Ag2C2, 
32C2H2. 

Decomp.  by  H2O.    Sol.  in  NH4OH+Aq. 

Insol.  in  alkalies.  (Bhaduri,  Z.  anorg.  1913, 
79  356  ) 

7Na2S2O3,  5Ag2S2O3,  86Ag2C2,  13C2H2. 
(Bhaduri.) 

Silver  sodium  thiosulphate  ammonia, 

NaAgS2O3,  NH3. 
Very  unstable.     (Schwicker,  B.  22.  1736.) 

Silver    strontium    thiosulphate,    Ag2S2O3, 

SrS2O3. 

Nearly  insol.  in  H2O.  Very  si.  sol.  in 
SrS2O3+Aq;  easily  sol.  in  NH4OH+Aq. 
(Herschel.) 

Sodium  thiosulphate,   Na2S2O3  and    +1,   2 

and  5H2O. 
100  pts.  H2O  dissolve: 

At  16°,  65  pts.  Na2S2O3. 
"20°,  69 
"25°,  75 
"30°,  82 
"35°,  89 
"40°,  98 
"  45°,  109 
"47°,  114 

(Mulder.) 

100  pts.  H2O  dissolve  at  0°,  47.6  pts. 
Na2S2O3;  at  20°,  69.5  pts.  ;  at  4~0*°,  104  pts.  ; 
at  60°,  192.3  pts.  (Kremers,  Pogg.  99.  50) 

100   pts.    H2O   dissolve    171    pts.    cryst. 
( =  108.9  pts.  anhydrous  )salt  at  19.5°  to  form 
a  solution  of  1.3875  sp.  gr.     (Schiff,  A.  113. 
350.) 

By  supersaturation  100  pts.  H2O  may  dis- 
solve 217.4  pts.  Na2S2O3  at  0°.  (Kremers.) 

Solubility  in  H2O. 


t° 

%  Na2S2O3 

Solid  phase 

0 

34.43 

Na2S2O3+5H2O 

10 

37.89 

tt 

20 

41.17 

(i 

30 

45.86 

tt 

40 

50.65 

a 

45 

54.49 

t( 

50 

62.92 

Na2S2O3+2H2O 

60 

67.39 

te 

72 

70.39 

{( 

80.5 

71.33 

tt 

90.5 

71.76 

it 

100 

72.68 

it 

(Taylor,  Proc.  Edinburgh  Soc.  1898,  22.  49.) 


Solubility  of  anhydrous  Na2S2O3  in  H2O  at  tc 


t° 

g.  Na  S2O3  per  100  g. 

Solution 

HO 

40 

67.40 

206.70 

45 

67.60 

208.60 

50 

67.76 

210.20 

55 

68.15 

214.00 

60 

68.48 

217.30 

65 

68.80 

220.50 

70 

69.05 

223.10 

75 

69.35 

226.30 

80 

69.80 

231.80 

(Young  and  Burke,  J.  Am.  Chem.  Soc.  1906, 
28.  327.) 


The  solubility  of  the  hydrates  of  Na2S2O3 
are  exceedingly  complicated.  There  are  five 
groups  of  hydrates,  (I)  primary,  (II)  second- 
ary, (III)  tertiary,  (IV)  quaternary,  and  (V), 
quintary,  and  transitions  occur  between  mem- 
bers of  the  same  and  different  groups. 
Na2S2O3+5H2O(I)  is  the  commercial  thio- 
sulphate. The  relations  and  solubility  of  the 
various  hydrates  is  shown  in  the  following 


akj^o^/r 

Solubility  of  Na2S203  in  H2O  at  t°. 

I.  Primary  hydrates. 

g.  Na2S2Os  per 

t° 

100  g. 

Solid  phase 

Solution 

H2O 

0 

33.40 

50.15 

Na2S203,  5H,0(I) 

5 

35.33 

54.64 

" 

10 

37.37 

59.69 

(C 

15 

39.11 

64.22 

{{ 

20 

41.20 

70.07 

(( 

25 

43.15 

75.90 

It 

30 

45.19 

82.45 

11 

35 

47.71 

91.24 

" 

40 

50.83 

105.37 

a 

45 

55.33 

123.87 

a 

48.17 

"    +Na2S203,  2H,0(I) 

0 

52.73 

111.60 

Na2S203,  2IT20(I) 

5 

53.45 

114.90 

R 

10 

53.94 

117.10 

t( 

20 

55.15 

122.68 

ii 

25 

56.03 

127.43 

tt 

30 

57.13 

133.27 

( 

40 

59.38 

146.20 

( 

'45 

60.73 

154.70 

t 

50 

62.28 

165.11 

c 

55 

63.85 

176.60 

t 

60 

65.68 

191.30 

( 

65 

68.04 

212.90 

t 

66.5 

... 



"     +Na2S203 

THIOSULPHATE,  SODIUM 


1069 


Solubility  of  Na2S2O3  in  H2O  at  t0.— 
Continued. 
II.  Secondary  hydrates. 

Solubility  of  Na2S2O3  in  H2O  at  t°  — 
Continued. 
IV.  Quaternary  hydrate. 

t° 

g.  NaiSzOs  per 
100  g. 

Solid  phase 

t° 

g.  NaaS2O3  per 
100  g. 

Solid  phase 

Solu 
tion 

H20 

Solu- 
tion 

H20 

0 
5 
10 
15 
20 
25 
30 
30.22 

41.96 
43.56 
45.25 
47.27 
49.38 
52.15 
56.57 

72.30 
77.17 

82.65 
89.36 
97.55 
108.98 
130.26 

Na2S2O,,  5H2O(II) 

t 
t 

.  i 
t 

"    Na2S2O3,  4H2O(II) 

0 
5 
10 
15 
20 
25 
30 
35 
40 
45 
50 
55 
58 

57.63 
58.08 
58.49 
59.00 
59.57 
50.35 
61.03 
61.94 
62.95 
64.22 
65.45 
67.07 

136.00 
138.60 
140.90 
143.90 
147.30 
152.30 
156.60 
162.80 
169.90 
179.50 
189.50 
203.70 

NaAO,,4ViH,0(IV) 

1C 

(( 
It 
It 
tt 

(t 
tl 
11 
tt 
tt 

,"     +Na2S203 

33.5 
36.2 
38.6 
40.65 

58.59 
60.51 
62.80 

141.48 
153.23 
168.82 

Na2S203,  4H2O(II) 
t( 

u 
"     +Na2S203,  H,0(II) 

0 
5 
10 
15 
20 
25 
30 
35 
40 
45 
50 
55 
56.5 

60.47 
60.74 
61.04 
61.57 
62.11 
62.73 
63.56 
64.32 
65.22 
66.02 
66.82 
67.90 

153.00 
154.70 
156.70 
160.20 
163.90 
168.30 
174.40 
180.20 
187.60 
194.30 
201.40 
211.50 

Na2S203,(H20(lI) 

a 
n 
a 
(i 
ft 

1C 

(I 
tl 
(( 
(I 

"     +Na2S203 

V.  Quintary  hydrates. 

0 
5 
10 
15 
20 
25 
30 
35 
27.5 

57.63 
58.23 
59.05 
60.02 
61.02 
62.30 
63.56 
65.27 

136.00 
139.40 
144.20 
150.10 
156.50 
165.30 
174.40 
188.00 

Na2S203,(2H20(V) 

< 
i 
< 

i 

( 

11  +Na2S203,  H20(V) 

30 
35 
40 
45 
50 
55 
43 

63.34 
64.07 
64.75 
65.58 
66.58 
67.59 

172.80 
178.40 
183.70 
190.50 
199.20 
208.50 

Na2S203/(H20(V) 

ti 
ti 
it 

"+Na2S203,  V«H,0(V) 

III.  Tertiary  hydrates. 

0 

5 
10 
13 
14.35 
14.3 

46.14 

48.44 
51.66 
54.96 

85.67 

93.95 
106.80 
122.00 

Na2S2O3,  6H2O  (III  and 

IV) 
u 
n 
ti 

"+Na,S,0,,  4/3H20(IV) 
"+Na2S2O3,  3/2H2O(lII) 

25 
35 
40 
45 
50 
55 
60 
65 
70 
70 

64.21 
64.60 
64.99 
65.61 
66.02 
66.57 
67.40 
68.24 
69.06 

179.40 
182.50 
185.60 
190.82 
194.30 
199.10 
206.70 
214.90 

Na2S203,  ^H20(V) 
tt 
ti 
i 
t 
i 

i 
t 

"    Na2S208 

0 
5 
10 
15 
20 
25 
30 
35 
40 
45 
47.5 
48.5 

57.42 
57.84 
58.28 
58.80 
59.28 
60.18 
60.78 
61.57 
62.60 
63.97 
64.68 

134.80 
137.20 
139.70 
142.70 
145.60 
151:10 
155.00 
160.20 
167.40 
177.50 
183.00 

Na2S203,  y«H,0(III) 

n 
K 
.                tt 
a 
(( 
te 
(t 
n 
« 

"  +Na2S203,  H,0(III) 

(Young  and  Burke,  J.  Am.  Chem.  Soc.  1906, 
28.  321.) 

Heat  is  absorbed  bv  dissolving  in  H2O. 
110   pts.    Na2S2O3+5H2O  +  100   pts.   H2O 
lower  temp,  from  10.7°  to  8°.     (Riidorff,  B. 
3.  68.) 
-f  i^H2O.      (Young   and   Burke,    J.   Am. 
Chem.  Soc.  1906,  28.  321.) 
+H20. 
+4/3H2O.    (Young  and  Burke.) 
+3/2H2O.    (Young  and  Burke.) 

47.5 
50 
52.5 
55 
60 
61 

64.78 
65.30 
65.89 
66.45 
68.07 

183.90 
188.20 
193.20 
198.10 
213.10 

Na2S2O3,  H2OaiI) 
tt 

a 
(t 
it 

"     +Na2S203 

1070 


THIOSULPHATE,  SODIUM  THALLOUS 


+2H2O. 

+4H2O.  M.-pt.  41.60°.  (Young  and 
Burke.) 

+5H2O.  M.-pt.  45°  (Kopp);  48°  (Krem- 
ers),  50°  (Mulder);  48.5°  (Tilden,  Chem.  Soc. 
46.  409);  47.9°  (Taylor,  Proc.  Edinburgh, 
Soc.  1898,  22.  249);  48.09°  (Richards  and 
Churchill,  Z.  phys.  Ch.  1899,  28.  314);  48.45° 
(Young  and  Burke,  J.  Am.  Chem.  Soc.  1906, 
28.  324.) 

Labile  modification  melts  at  32°.  (Parmen- 
tier  and  Amat,  C.  R.  98.  735.) 

Sp.  gr.  of  Na2S2O3+Aq  at  19°. 
%  =  %Na2S2O3+5H2O. 


Sodium  thallous  thiosulphate,  3Na2S203, 
2T12S2Q3+10H2O. 

Sol.  in  H2O.    (Werther.) 

+8H2O.     (Jochum.) 

2Na2S2O3,  T12S2O3+8H2O.  (Vortmann 
ind  Padberg,  B.  22.  2638.) 

Sodium  zinc  thiosulphate,  Na2S2O3,  2ZnS2O3 

+23H2O. 

Sol.  in  H2O.  (Jochum,  C.  C.  1885.  642.) 
3Na2S2O3.  2ZnS2O3'+10H2O.  Deliques- 
cent. (Vortmann  and  Padberg,  B.  22.  2640.) 

Sodium  thiosulphate  mercuric  iodide, 


% 

Sp.  gr. 

% 

Sp.  gr. 

% 

Sp.  gr. 

^ixj*202vy3,  iigj.2. 

Decomp.  by  H2O  and  by  alcohol.     (Eder 

1 

1.0052 

18 

1.0975 

35 

1.1986 

and  Ulm,  M.  1882,  3.  197.) 

2 
3 

1.0105 
1.0158 

19 

20 

1.1031 
1  .  1087 

36 
37 

1.2048 
1.2110 

Strontium  thiosulphate,   SrS2O3+5H2O. 

4 

1.0211 

21 

1.1145 

38 

1.2172 

Permanent.    Sol.  in  6  pts.  cold  H2O  (Gay- 

5 

1.0264 

22 

1  .  1204 

39 

1.2234 

Lussac);  in  4  pts.  H2O  at  13°,  and  1.75  pts. 

6 

1.0317 

23 

1.1263 

40 

1.2297 

boiling  H2O  (HerscheL  1819). 

7 

1.0370 

24 

1.1322 

41 

1.2362 

1  g.  is  sol.  in  3.7  cc.  H2O  at  room  temp. 

8 

1.0423 

25 

1  .  1381 

42 

1.2427 

Antenrieth,  Z.  anal.  1898,  37.  293.) 

9 

1.0476 

26 

1  .  1440 

43 

1.2492 

Gradually  efflorescent.     Insol.  in  alcohol. 

10 

1.0529 

27 

1.1499 

44 

1.2558 

HerscheL) 

11 

1.0584 

28 

1  .  1558 

45 

1.2624 

12 
13 
14 
15 
16 

1.0639 
1.0695 
1.0751 
1.0807 
1.0863 

29 
30 
31 
32 
33 

1.1617 
1  .  1676 
1  .  1738 
1  .  1800 
1  .  1862 

46 
47 
48 
49 
50 

1.2690 
1.2756 
1.2822 

1.2888 
1.2954 

Thallous  thiosulphate. 

Ppt.    SI.  sol.  in  cold,  easily  sol.  in  hot  H2O. 
Crookes.) 
Easily   sol.   in   Na2S2O3+Aq.      (Jochum.) 

17 

1.0919 

34 

1  .  1924 

Tin  thiosulphate  (?). 

(Schiff,  A.  113.  118.) 

Sol.  in  H2O. 

B.-pt.  of  Na2S2O3+Aq.    P  =  pts.  Na2S2O3  to 
100  pts.  H2O. 

Uranyl  thiosulphate,  (UO2)S2O3. 

Ppt.    (Faktor.  C.  C.  1901,  II.  878.) 

B.-pt.  1      P 

B.-pt. 

p 

B.-pt.          P 

101°     14 
102      27 
103      39 

110° 
111 
112 

104 
113 
122 

119°     201 
120      214.5 
121      229 

Zinc   thiosulphate,    ZnS2O3+zH2O. 
Very  deliquescent,  and  very  sol.  in  H2O 
and  alcohol.    (Rammelsberg.) 

104      49  .  5 

113 

131.5 

122      244 

105      59 

114 

141.5 

123       262 

Zinc  thiosulphate  ammonia,   ZnS2O3,  2NH3. 

106      68 

115 

152 

124      283 

Decomp.  by  H2O.     Sol.  in  NH4OH+Aq, 

107      77 

116 

164 

125      311 

from  which  it  is  pptd.  by  alcohol.     (Rammels- 

108     86 

117 

175.75 

126      348 

berg,  Pogg.  66.  62.) 

109      95 

118 

188 

(Gerlach,  Z.  anal.  26.  436.) 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  829.) 

100  pts.  absolute  ethyl  alcohol  dissolve 
at  room  temperature  2.5  mg.  Na2S2O< 
(Bodtker,  Z.  phys.  Ch.  1897,  22.  410.) 

100   pts.    absolute   ethyl   alcohol   dissolve 
at    room    temperature    3.4    mg.    Na2S2O3 
5H2O.     (Bodtker,  Z.  phys.  Ch.  1897,  22.  510.; 

Sol.  in  oil  of  turpentine  (Edison,  Am 
Chemist,  7.  127).  Insol.  therein  (Techn 
J.  B.  27.  1003). 

Insol.  in  ethyl  acetate.  (Casaseca,  C.  R 
30.  821.) 


Decamp.  H2O  and  alkalies. 
Stable  in  the  air.    (Muthmann,  B.  1897,  30. 
630.) 


Thkx&thiazyl  ^'chloride,  S3N2C12. 
See  Nitrogen  sulphochloride. 

ThioZnthiazyl  chloride,  S4N3C1. 
See  Nitrogen  sulphochloride. 

Thio^nthiazyl  iodide,  N3S4I. 

Decomp.  spontaneously  in  the  air. 
unstable.      (Muthmann,   B.    1897,   30. 


Very 

631.) 


THORIUM  HYDRIDE 


1071 


ThioZnthiazyl  nitrate,  S4N8NO8. 

Sol.  in  H2O  with  decomp.  Sol.  in  HNO3  + 
Aq.  (Demargay,  C.  R.  91.  1066.) 

Sol.  in  cold  H2O  with  decomp. 

Completely  insol.  in  organic  solvents,  as 
CS2,  CHC13,  acetone,  and  acetic  ether. 
(Muthmann  and  Seitter,  B.  1897,  30.  629.) 

ThioZhthiazyl  sulphate  (S4N8)HSO4. 

Stable  on  air.  Sol.  in  H2O  with  decomp. 
(Demarcay,  C.  R.  91.  854.  1066.) 

ThioJn'thiazyl  sulphocyanide,  N3S4CNS. 

Stable  in  the  air. 

Sol.  in  benzene  and  chloroform.  (Muth- 
mann and  Seitter,  B.  1897,  30.  631.) 

Dithiotefrathiazyl  bichloride,  S6N4C12. 
See  Nitrogen  sulphochloride. 

Thorium,  Th. 

Not  oxidised  by  boiling  H2O. 

Quickly  sol.  (Chydenius,  Pogg.  119.  43), 
very  slowly  sol.  by  long  boiling  (Berzelius, 
Pogg.  16.  385)  in  HNO3+Aq.  Insol.  in  cold, 
easily  sol.  in  warm  dil.  H2SO4+Aq.  Slowly 
sol.  in  cold,  rapidly  in  hot  HCl+Aq.  Easily 
oxidised  by  aqua  regia.  Insol.  in  KOH+Aq 
or  HF+Aq.  ' 

SI.  sol.  in  dil.  H2SO4+Aq;  decomp.  by 
cone.  H2SO4.  Very  si.  sol.  in  dil.,  and  less  in 
cone.  HNO3+Aq.  Easily  sol.  in  cone.  HC1  + 
Aq,  and  aqua  regia.  (Nilson,  B.  16.  2521.) 

Thorium  B. 

Somewhat  sol.  in  hot  H2O,  which  dissolves 
70%  in  an  hour.  More  rapidly  sol.  in  dil 
acids  or  hot  KI-f-Aq.  Somewhat  sol.  in 
organic  solvents.  Insol.  in  CS2  and  in  methy 
lene  iodide.  (Hogley,  Phil.  Mag.  1913,  (6 
26.  331.) 

Thorium  C. 

Somewhat  sol.  in  hot  H2O.  More  rapidly 
sol.  in  hot  KI+Aq.  and  in  dil.  acids.  More 
sol.  in  organic  solvents  than  thorium  B 
20%  sol.  in  CS2  or  methylene  iodide  in  1< 
minutes.  (Hogley,  Phil.  Mag.  1913,  (6)  25 
331.) 

Thorium  teZraboride,  ThB4. 

Sol.  in  cold  cone.  HNO3  and  HC1  and  in  ho 
cone.  H2SO4.  (Jassonneix,  C.  R.  1905,  141 
192.) 

Thorium  fozaboride,  ThBr6. 

Sol.  in  hot  dil.  or  cone.  HNO3;  insol.  ic 
H2SO4,  HC1,  HF  and  aq.  alkalies.  (Jasson 
neix,  C.  R.  1905,  141.  193.) 

Thorium  cfabromide,  ThBr2. 

Sol.  in  H2O  with  partial  decomp.  (Troos 
and  Ouvrard,  A.  ch.  (6)  17.  227.) 


Thorium  teirabromide,  ThBr4. 

Sol.  in  H2O.     (Berzelius.) 

Very  hygroscopic,  and  sol.  in  H2O  with 
artial  decomp.  (Troost  and  Ouvrard.  A. 
h.  (6)  17.  229.) 

SI.  sol.  in  organic  solvents.  (Matthews, 
.  Am.  Chem.  Soc.  1898,  20.  840.) 

+7H2O.  Sol.  in  alcohol.  (Rosenheim,  B. 
900,  33.  979.) 

+8H2O.  Very  sol.  in  alcohol  and  H2O. 
nsol.  in  chloroform  and  light  petroleum. 
Lesinsky,  Z.  anorg.  1897,  15.  82.) 

Thorium     feZrabromide     ammonia,     ThBr4, 

3NH3. 

Insol.  in  organic  solvents.  (Matthews,  J. 
Am.  Chem.  Soc.  1898,  20.  840.) 

Thorium  carbide,  ThC2. 

Almost  insol.  in  cone,  acids;  decomp.  by 
H2O  and  by  dil.  acids.  (Moissan,  C.  R. 
1896,  122.  577.) 

Thorium  fefrachloride,  ThCl4. 

Anhydrous.  Extremely  deliquescent,  and 
sol.  in  H2O  with  evolution  of  heat.  Sol.  in 
alcohol. 

Sol.  in  ether.  (Matthews.  J.  Am.  Chem. 
Soc.  1898,  20.  824.) 

+7H2O.  Deliquesces  in  the  air.  Very  sol. 
in  H2O  and  alcohol.  Insol.  in  ether.  (Kriiss, 
Z.  anorg.  1897,  14.  368.) 

+8H2O.  Hydroscopic.  Easily  sol.  in  H2O 
and  absolute  alcohol.  Not  pptd.  from  solution 
in  alcohol  by  ether. 

+9H2O.  As  above.  (Rosenheim,  Z. 
anorg.  1903,  36.  426.) 

Thorium  tefrachloride  ammonia,  ThCl4, 6NH8. 

Insol.  in  ether.    Decomp.  by  H20. 

ThCl4,  8NH3.  Fumes  in  moist  air.  De- 
comp. by  H2O.  (Matthews,  J.'Am.  Chem. 
Soc.  1898,  20.  824.) 

The  compds.  of  ThCl4  with  NH3  are  of  the 
type  ThCh,  nNH3  and  may  be  classified  into 
three  groups. 

(1)  n  =  4,  6,  7,  12,  18.     Compds.  are  de- 
comp. by  H2O. 

(2)  n  =4,  6,  7.    Compds.  are  not  decomp.  by 
H2O. 

(3)  n  =  6,  7,  12,  18.    The  first  two  compds. 
of  this  series  are  identical  with  the  last  two  of 
group  (2). 

ThCl4,  4NH3  of  group  (2)  is  the  only  one  in 
the  whole  series  stable  above  120°.  (Chauve- 
net,  C.  R.  1910,  151.  387.) 

Thorium  fluoride,  ThF4+4H2O. 
Insol.  in  H2O  or  HF+Aq. 


Thorium  hydride,  ThH2. 

Decomp.  by  dil.  HCl+Aq. 
24.  873.) 


(Winkler,  B. 


1072 


THORIUM  HYDROXIDE 


Thorium  hydroxide,  Th(OH)4. 

Insol.  in  H2O. 

Sol.  in  acids,  except  oxalic,  molybdic,  and 
hydrofluoric  acids. 

Insol.  in  alkali  hydroxides,  but  easily  sol 
in  alkali  carbonates +Aq.  More  sol.  in 
NH4OH+(NH4)2CO3+ Aq  thanin  (NH4)2CO3 
+Aq.  alone.  (Berzelius.)  Not  pptd.  in 
presence  of  tartaric  and  citric  acids.  (Chyde- 
nius,  Pogg.  119.  43.) 

4ThO2.  H2O.  Insol.  in  water  and  acids  at 
boiling  temp. 

Thorium  hydroxybromide,  Th(OH)2Br2+ 

11H2O. 

Sol.  in  alcohol.  (Rosenheim,  B.  1900,  33. 
979.) 

Thorium  hydroxychloride,    (OH)ThCl3+ 
11H2O. 

Sol.  in  alcohol.  (Rosenheim,  B.  1900,  33. 
978.) 

Th(OH)2Cl2+5H2O.  Slowly  takes  up  H2O 
from  the  air. 

Sol.  in  H2O  without  decomp. 

Sol.  in  alcohol.  Pptd.  from  solution  in 
alcohol  by  ether.  (Rosenheim,  Z.  anorg. 
1903,  36.  425.) 

+8H20.  Hydroscopic;  sol.  in  alcohol. 
(Rosenheim,  B.  1900,  33.  978.) 

Thorium  hydroxyiodide,  Th(OH)I8+10H2O. 

Evolves  iodine  in  the  light.  (Rosenheim, 
Z.  anorg.  1903,  35.  430.) 

Thorium  iodide. 
Sol.  in  H2O. 

Thorium  nitride,  Th,N4. 

Decomp.  by  H2O.  (Matignon,  C.  R.  1901, 
132.  37.) 

Thorium  oxide,  ThO2. 

When  ignited  is  insol.  in  HC1,  and  HNO3+ 
Aq.  Sol.  in  H2SO4  by  heating  to  boiling  and 
subsequent  addition  of  H2O.  Insol.  in  alkali 
hydrates  or  carbonates +Aq. 

Thorium  wetoxide,  Th306+H2O. 

SI.  sol.  in  HC1.  (Locke,  Z.  anorg.  1894,  7. 
348.) 

+2H2O.  Loses  1  H2O  at  100°.  Sol.  in 
H2O;  insol.  in  NH4OH+Aq.  (Locke.) 

Metathorium  oxide. 

Sol.  in  H2O  after  having  been  treated  with 
cone.  HNO3  or  HCl+Aq,  even  if  previously 
ignited. 

ThO2,zTh(OH)4.  Compare  Th3O5.  (Locke) 
(Stevens,  Z.  anorg.  1901,  27.  42.) 

Thorium  peroxide,  Th2O7. 

Precipitate.    (Cleve,  C.  R.  100.  605.) 


Thorium  oxychloride. 

Decomp.  by  H2O  into  ThCl4  and  ThO3. 

ThOCla.    Sol.  inH2O. 

Insol.  in  abs.  alcohol.  (Matignon,  A.  ch. 
1907,  (8)  10.  133.) 

+3H2O. 

+5H2O.  (Matignon,  A.  ch.  1907,  (8)  10. 
135.) 

Metothorium  oxychloride,  ThO2,  zThC!4. 

Hydroscopic;  sol.  in  H2O;  insol.  in  abs. 
alcohol.  (Stevens,  Z.  anorg.  1901,  27.  47.) 

Thorium  oxyfluoride,  ThOF2. 

Insol.  in  H2O. 

Sol.  in  H2SO4  with  decomp.  (Chauvenet, 
C.  R.  1908,  146.  974.) 

Thorium  oxysulphide,  ThS2,  2ThO2. 

(Chydenius.) 

Thorium  phosphide. 

Insol.. in  H2O.     (Berzelius.) 

Thorium  silicide,  ThSi2. 

Sol.  in  aq.  min.  acids;  insol.  in  aq.  alkalies-. 
Decomp.  by  fusion  with  NaOH  or  KOH. 
(Honigschmid,  C.  R.  1906,  142.  158.) 

Thorium  sulphide,  ThS2. 

Insol.  in  warm  H2SO4.  Very  slightly  at- 
tacked by  HNO3  or  HCl+Aq.  Sol.  in  hot 
aqua  regia.  (Berzelius.) 

Thoromolybdic  acid. 

Ammonium  thoromolybdate, 

(NH4)8Th(Mo207)6+8H20. 

Insol.  in  H2O;  sol.  in  dil.  acids.  (Barbieri, 
C.  A.  1913.  372*.) 

(NH4)6H2Th(Mo2O7)6+llH2O.  Insol.  in 
H2O;  sol.  in  dil.  acids.  (Barbieri.) 

Silver  thoromolybdate,  Ag8Th(Mo2O7)6. 

Insol.  in  H?O;  si.  sol.  in  HNO3+Aq,  but 
nearly  insol.  in  presence  of  AgftO3.  (Bar- 
bieri.) 

Sodium   thoromolybdate,   Na8Th(Mo207)6+ 
15H2O. 

Insol.  in  H2O;  sol.  in  dil.  acids.    (Barbieri.) 
Na6H2Th(Mo2O7)6+17H2O.    Insol.  in  H20; 
sol.  in  dil.  acids.    (Barbieri.) 

Thulium,  Tm. 

Thulium  chloride,  Tm2Cle+14H20. 

Very  sol.  in  H2O  and  in  alcohol.  (James, 
J.  Am.  Chem.  Soc.  1911,  33.  1342.) 

Thulium  hydroxide. 

Easily  sol.  in  dil.  acids.  (James,  J.  Am. 
Chem.  Soc.  1911,  33.  1342.) 


TIN  BROMIDE,  BASIC 


1073 


Thulium  oxide,  Tm2O3. 

Slowly  sol.  in  hot  cone,  acids.  (James, 
J.  Am.  Chem.  Soc.  1911,  33.  1342.) 

Tin,  Sn. 

Insol.  in  H2O.  Tin  is  not  atacked  by  dis- 
tilled H2O  when  air  is  passed  through  it  for  a 
week. 

Slowly  sol.  in  dil.  cold  HCl+Aq,  but 
rapidly  sol.  if  hot  and  cone.  Slowly  sol.  in 
hot  dil.  H2SO4+Aq,  but  decomp.  by  hot 
cone.  H2SO4. 

Readily  sol.  in  cold  aqua  regia.  Attacked 
violently  by  cone.  HNO3+Aq  with  pptn.  of 
SnO2.  Completely  sol.  in  dil.  cold  HNO3+ 
Aq  (1  pt.  HNO3:  1  pt.  H2O)  at  22°.  (Hay, 
C.  N.  22.  298.)  Not  attacked  by  pure  cone. 
HNO3+Aq  of  1.512-1.419  sp.  gr.,  but  vio- 
lently attacked  by  less  cone.  acid.  Also  at- 
tacked by  most  cone,  acid  if  it  contains  NO2. 
(Millon,  A.  ch.  (3)  6.  95.) 

If  Sn  is  placed  in  dil.  HNO3+Aq  of  1.15  sp. 
gr.  it  is  si.  dissolved,  but  soon  pptd.  again  as 
SnO2.  If  a  small  amt.  of  NH4C1  is  added,  the 
Sn  remains  permanently  in  solution;  HC1+ 
Aq  has  a  similar  action.  (Ordway,  Am.  J. 
Sci.  (2)  23.  220.)  Easily  sol.  in  the  cold  in 
mixture  of  1  vol.  H2SO4,  2  vols.  HNO3,  and  3 
vols.  H2O.  (Basset,  C.  N.  63.  172.) 

HNOs+Aq  containing  less  than  12%  HNO3 
attacks  Sn  and  forms  a  stannous  salt,  which 
decomposes,  giving  a  turbid  solution.  HNO3 
+Aq  (12-45%  HNO3)  completely  dissolves 
Sn,  but  solution  becomes  turbid  on  standing. 
HNO3+Aq  containing  more  than  45%  HNO3 
does  not  dissolve  Sn,  but  forms  a  white  sub- 
stance, which  is  sol.  in  H2O  if  over  70%  acid 
is  used;  this  solution  soon  becomes  turbid. 
(Montemartini,  Gazz.  ch.  it.  22.  384.) 

Sn  dissolves  in  HNO3+Aq  at  low  temps. 
(0-21°).  When  very  dil.  HNO3+Aq  (14% 
HNO3)  is  used,  the  amount  of  stannous  salt 
formed  decreases  only  slightly  with  increase 
of  temp,  while  with  30-40%  acid  it  falls  to 
zero  at  21°.  (Walker,  J.  Soc.  Chem.  Ind. 
1893.  845.) 

In  presence  of  Fe,  Cr  or  Al,  HNO8+Aq 
acts  on  Sn  to  form  soluble  products,  from 
which  cone.  HNO3  ppts.  all  Sn  as  meta- 
stannic  acid,  (van  Leent,  C.  C.  1899, 1. 101.) 

Much  more  sol.  in  acids  when  small  quanti- 
ties of  metallic  salts  have  been  added.  This 
is  most  noticeable  when  PtCl4  or  tartar  emetic 
is  added  to  HCl+Aq.  HCl+Aq  with  tartar 
emetic  exerts  11  times,  and  with  PtCl4  13 
times  the  action  exhibited  by  pure  acid. 
(Millon,  C.  R.  21.  47.) 

Sol.  in  2N  HClOs+Aq.  (Hendrixson,  J. 
Am.  Chem.  Soc.  1904,  26.  755.) 

Pyrosulphuric  acid  dissolves  Sn  on  warm- 
ing. (Divers,  Chem.  Soc.  1885,  47.  639.) 

Hot  telluric  acid  attacks  Sn.  (Hutchins, 
J.  Am.  Chem.  Soc.  1905,  27.  1183.) 

Sn  is  attacked  by  17%  HN3+Aq.  (Cur- 
tius  and  Rissom,  J.  pr.  1898,  (2)  58.  299.) 

Sol.  in  a  solution  of  Na  in  liquid  NH3. 


(Kraus,  J.  Am.  Chem.  Soc.  1907,  29.  1562.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  830.) 

Sol.  in  boiling  alum+Aq  (1  pt.  alum  to  4 
pts.  H20). 

Sol.  in  KHSO3,  NH4C1  (1 :4),  and  K2C4H4O6 
+Aq.  SI.  sol.  in  KC2H3O2+Aq,  but  not  at- 
tacked by  MgSO4,  K2SO4,  KNO3,  or  Na2SO4 
+Aq.  (Cludius,  J.  pr.  9.  161.) 

Sol.  in  alkalies +Aq. 

Attacked  easily  by  cone.  NaCl,  KC1,  or 
NH4NO3+Aq;  not  attacked  by  NH4Cl+Aq. 
(Hallock,  Am.  Ch.  J.  6.  52.) 

Sol.  in  Fe(NO3)3+Aq  in  presence  of  HNO3 
+Aq  in  proportion  of  1  atom  Sn  to  1  atom  Fe. 
(Lepez  and  Storch,  W.  A.  B.  98,  2t>.  268.) 

Solubility  in  dil.  saline  solutions. 

100  ccm.  H2O  containing  0.5  g.  NaCl  or 
KC1  dissolve  6  mg.  Sn  from  11.8  sq.  cm.  in  one 
week  when  air  without  CO2  is  passed  through 
the  solution,  but  none  at  all  when  the  air  con- 
tains CO2. 

100  ccm.  H2O  containing  1  g.  NH4C1  dis- 
solve 5  mg.  Sn  under  above  conditions  with- 
out CO2,  and  none  with  CO2. 

With  1  g.  MgCl2,  1  mg.  Sn  was  dissolved 
without  CO2,  and  none  wijth  CO2. 

With  1  g.  K2SO4,  2  mg.  Sn  were  dissolved 
without  CO2,  and  none  with  CO2. 

With  1  g.  KNO3,  3  mg.  Sn  were  dissolved 
without  CO2,  and  1  mg.  with  CO2. 

With  1  g.  Na2C03,  7  mg.  Sn  were  dissolved 
without  CO2. 

With  1  g.  NaOH,  220  mg.  Sn  were  dis- 
solved without  CO2. 

CaO2H2+Aq  did  not  dissolve.  (Wagner, 
Dingl.  221.  260.) 

Not  attacked  by  sugar +Aq.  (Klein,  C.  R. 
102.  1170.) 

%  ccm.  oleic  acid  dissolves  0.0134  g.  Sn 
in  6  days.  (Gates,  J.  phys.  Chem.  1911,  15. 
143.) 

Tin  antimonide,  SnSb. 

(Stead,  J.  Soc.  Chem.  Ind.  1897,  16.  205.) 

Tin  arsenide,  Sn3As2. 

(Stead,  J.  Soc.  Chem.  Ind.  1897,  16.  206.) 

Tin  (stannous)  bromide,  SnBr2. 

Sol.  in  H2O. 

Sol.  in  pyridine.  (Naumann,  B.  1904,  37. 
4609.) 

Mol.  weight  determined  in  pyridine  and 
ethyl  sulphide.  (Werner,  Z.  anorg.  1897,  16. 
23.) 

Tin  (stannic)  bromide,  basic,  SrBr»OH+ 
3H20. 

Sol.  in  H20.  Decomp.  in  aq.  solution  when 
warmed. 

Sol.  in  ether,  methyl  alcohol,  ethyl  alcohol, 
acetone,  acetic  acid  and  esters  of  organic 
acids.  Nearly  insol.  in  benzene,  ligroin  and 
CHC13.  (Pfeiffer,  Z.  anorg.  1914,  87.  242.) 


1074 


TIN  BROMIDE 


Tin  (stannic)  bromide,  SnBr4. 

Deliquescent.  Sol.  in  H2O  without  evolu- 
tion of  heat.  (Balard.) 

Decomp.  by  H2O  much  more  quickly  than 
SnCl4.  (Lorenz,  Z.  anorg.  1895,  9.  378.) 

Easily  sol.  in  AsBr3.  (Walden,  Z.  anorg. 
1902,  29.  374.);  PC13,  PBr3  and  S2C12.  (Wal- 
den, Z.  anorg.  1900,  26.  217.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

+4H2O.  (Preis  and  Raymann,  C.  C.  1882. 
773.) 


Stannic  hydrogen  bromide,  SnBr4,  2HBr. 
See  Bromostannic  acid. 

Stannic  bromide  with  MBr. 
See  Bromostannate,  M. 


Tin  (stannic)  bromochloride,  SnClBr3. 

Fumes  in  moist  air;  decomp.  by  H2O.  (Bes- 
son, C.  R.  1897,  124.  685.) 

SnCl2Br2.  Fumes  in  moist  air.  Decomp.  by 
H2O.  (Besson.) 

SnCl3Br.  Fumes  in  moist  air.  Decomp.  by 
H2O.  (Besson.) 


Tin  (stannic)  bromoiodide,  SnBr2I2. 

Sol.  in  cold  H2O.    Decomp.  in  aq.  solution 
at  80°. 

SnBr3I. 

SnBrI3.    (Lenormand.  C.  C.  1899,  II.  521 
J.  Pharm.  1899,  10.  114.') 


Tin  (stannous)  chloride,  SnCl2,  and  +2H2O. 

Not  deliquescent.  100  pts.  H2O  dissolve 
83.9  pts.  SnCl2  at  0°.  (Engel,  A.  ch.  (6)  17 
347.)  100  pts.  H2O  dissolve  269.8  pts.  SnCl2 
at  15°,  and  sat.  solution  has  sp.  gr.  1.827 
(Michel  and  Krafft,  A.  ch.  (3)  41.  478.)  Sol 
in  a  certain  amount  of  H2O  without  decomp. 
but  more  H2O  causes  pptn.  of  SnO,  SnCl2. 

SnCl2+Aq  absorbs  O  from  air. 

Melts  in  crystal  H2O  at  46°.     (Ordway. 

Sat.  solution  boils  at  121.7°. 

Sp.  gr.  of  SnCl2+Aq  at  15°  containing: 

5  10  15  20  %  SnCl2+2H20 
1.0331  1.0684  1.1050  1.1442 

25  30  35  40  %  SnCl2+2H2O 
1.1855  1.2300  1.2779  1.3298 

45  50  55  60  %  SnCl2+2H2O 
1.3850  1.4451  1.5106  1.5823 

65         70         75  %  SnCl2+2H20. 
1.6598  1.7452  1.8399 

(Gerlach,  Dingl.  186.  131.) 


SnCl2 

HCl 

Sum  of 

Sp.   gr. 
of  solu- 

jj2O 

2 

equiv. 

tion 

74 

0 

74 

.532 

8.33 

66.7 

6.6 

73.3 

.489 

8.35 

63.75 

13.54 

77.29 

.472 

8.198 

68.4 

24.8 

93.2 

.524 

7.869 

81.2 

34.9 

116.1 

.625 

7  .  305 

94.2 

40.0 

134.2 

.724 

6.880 

117.6 

44 

161.6 

1.883 

6.108 

147.6 

49.4 

197.0 

2.114 

5.387 

156.4 

66 

222.4 

2.190 

4.715 

157 

78 

235 

2.199 

4.309 

Solubility  of  SnCl2  in  HCl+Aq. 


SnCL 


Yz  molecules  SnCl2  in  milligrammes  in 
10  com.  solution;  HC1  =  molecules  HC1  in 
milligrammes  in  ditto;  H2O  =  amt.  H2O 
present  in  grammes. 


(Engel,  A.  ch.  (6)  17.  347.) 

Solubility  is  thus  diminished  by  HCl+Aq, 
while  there  are  less  than  8-10  mols.  HC1  for 
mol.  SnCl2.  When  that  limit  is  passed  the 
solubility  rapidly  increases.  (Engel.) 

Sol.  in  very  dil.  HC1  or  tartaric  acid  +Aq. 
Sol.  in  KOH+Aq.  Sol.  in  cone.  SnOCl2+Aq. 
(Gerlach.)  Sol.  in  NH4Cl+Aq. 

Anhydrous  SnCl2  is  partially  sol.  in  liquid 
NH3.  (Gore,  Am.  Ch.  J.  1898,  20.  830.) 

Sol.  in  absolute  alcohol.  Insol.  in  oil  of 
turpentine. 

11.41  pts.  SnCl2  are  sol.  in  100  pts.  ether  at 
0°. 

11.38  pts.  SnCl2  are  sol.  in  100  pts.  ether 
at  16°.  . 

11.38  pts.  SnCl2  are  sol.  in  100  pts.  ether  at 
35.5°.  (Laszczynski,  B.  1894,  27.  2286.) 

Anhydrous  SnCl2  is  sol.  in  ether.  (de 
Jong,  Z.  anal.  1902,  41.  596.) 

1  g.  anhydrous  SnCl2  is  sol.  in  1.8  g.  acetone 
at  18°.  Sp.  gr.  of  sat.  solution  180/40  =  1.6. 
(Naumann,  B.  1904,  37.  4336.) 

Sol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

Anhydrous  SnCl2  is  sol.  in  methyl  acetate 
to  the  extent  of  15.7%.  (Schroder  and 
Steiner,  J.  pr.  1909,  (2)  79.  63.) 

31.20  pts.  SnCl2+2H2O  are  sol.  in  100  pts. 
ethyl  acetate  at— 2°. 

35.53  pts.  SnCl2+2H2O  are  sol., in  100  pts. 
ethyl  acetate  at  +22°. 

73.44  pts.  SnCl2+2H2O  are  sol.  in  100  pts. 
ethyl  acetate  at  82°.  (Laszczynski,  B.  1894, 
27.  2286.) 

1  pt.  anhydrous  SnCl2  is  sol.  in  22.40  pts. 
ethyl  acetate  at  18°.  D18°/4°  =0.9215. 
(Naumann,  B.  1910,  43.  319.) 

Insol.  in  ethyl  amine  (Shinn,  J.  phys. 
Ch.  1907,  11.  538);  pyridine  (Naumann, 
B.  1904,  37.  4609):  benzonitrile  (Naumann, 
B.  1914,  47.  1369.) 


TIN  CHLORIDE 


1075 


Insol.  in  CS».  (Arctowski,  Z.  anorg.  1894 
6.  257.) 

Sol.  in  urethane.  (Castoro,  Z.  anorg.  1899 
20.  61.) 

Mol.  weight  determined  in  pyridine  am 
ethyl  sulphide.  (Werner,  Z.  anorg.  1897 
15.  22.)  . 

Tin  (stannic)  chloride,  basic,  SnCl3OH+3H2O 

Hydroscopic. 

Sol.  in  H2O. 

Sol.  in  ether,  alcohol,  acetone,  acetic  acid 
Nearly  insol.  in  ligroin  and  benzene.  (Pfeiffer 
Z.  anorg,  1914,  87.  241.) 

Tin  (stannic)  chloride,  SnCl4. 

(a)  Ordinary  modification. — Deliquescent 
Sol.  in  H2O.  On  diluting  SnCl4+Aq  and 
boiling,  SnO2  separates  out.  SnCl4+Aq  is 
not  pptd.  by  HNO3,  HC1,  or  H2SO4+Aq 
H3PO4+Aq  ppts.  in  a  few  days,  and  H3AsO4  + 
Aq  in  a  short  time.  No  ppt.  is  formed  by 
K2SO4,  Na2SO4,  KC1,  NaCl,  NH4C1,  KNOl 
etc.  +  Aq. 


Sol.  in  S2C12.  (Walden,  Z.  anorg.  1900,  25. 
217.) 

Easily  sol.  in  PC13  and  PBr3.  (Walden, 
Z.  anorg.  1900,  25.  211.) 

Very  sol.  in  liquid  NH3.  (Gore,  Am.  Ch. 
J.  1899,  20.  830.) 

Very  sol.  in  absolute  alcohol,  from  which 
it  is  pptd.  by  H2O.  Easily  sol.  in  ether;  de- 
comp.  by  oil  of  turpentine.  Miscible  with 
CS2  and  Br2. 

Sol.  in  acetone.  (Naumann,  B.  1904,  37. 
4328.) 

Sol.  in  acetone  and  in  methylal.  (Eid- 
mann,  C.  C.  1899,  II.  1014.) 

Sol.  in  ethyl  acetone.  (Naumann,  B.  1904, 
37.  3601.) 

Distribution  of  SnCl4  between  H2O  and 
xylene. 

n  =  pts.  by  wt.  of  Cl  in  100  pts.  of  H2O 
layer. 

m  =  pts.  by  wt.  of  Cl  in  100  pts.  of  xylene 
layer. 

k  =  partition  coefficient. 

50  cc.  xylene+60  g.  SnCl4.5H2O. 


n 

m 

k 

SnCl4 
+5H2O 

Sp.  gr. 

SnCU 
+5H20 

Sp.  gr. 

SnCU 
+5H20 

Sp.  gr. 

66° 

40.35 

0.08 

504.4 

80° 

QQ    QK 

0  175 

228  5 

2 

1.012 

34 

1.226 

66 

.538 

97.5° 

40.24 

0.33 

122.1 

4 

1.024 

36 

00 

1.242 

1       OCQ 

68 

.563 

jro'r 

111° 

40.27 

0.68 

59.3 

8 

.048 

OO 

40 

1.276 

72 

.614 

(Smirnoff,  Z.  phys.  Ch.  1907,  68.  377.) 

10 

059 

42 

1.293 

74 

.641 

• 

12 

.072 

44 

1.310 

76 

.669 

50  cc.  xylene+60  g.  SnCl4.4H2O. 

14 

.084 

46 

1.329 

78 

1.698 

16 

.097 

48 

1.347 

80 

1.727 

t 

18 
20 
22 

.110 
.124 
.137 

50 
52 
54 

1.366 
1.386 
1.406 

82 
84 
86 

1.759 
1.791 
1.824 

66° 
80° 
100° 

41.905 
41.915 
41  845 

0.925 
1.555 
2  515 

45.3 
27.0 
16  7 

24 
26 

1.151 
1.165 

56 

58 

.426 
.447 

88 
90 

1.859 
1.894 

111° 

41.68 

3.235 

12.9 

28 

1.180 

60 

.468 

92 

1.932 

(Smirnoff.) 

30 

1.195 

62 

.491 

94 

1.969 

32 

1.210 

64 

.514 

95 

1.988 

50  cc.  xylene+60  g.  SnCl4.3H2O. 

(Gerlach,  Dingl.  178.  49.) 

t° 

n 

m 

k 

Sp.  gr.  of  SnCl4+Aq. 

80° 

43.205 

9.95 

4-4 

Deg. 

Baum6 

%  Sn 

Deg. 

Baum6 

%  Sn 

Deg. 

Baum£ 

%  Sn 

94° 
100° 

42  .  545 
42.645 

.325 
10.56 

.6 
5.1 

111° 

42  31 

10.03 

4.2 

65.7 
65 

29.45 
29.12 

55 
54 

24.47 
24.02 

34 
33 

14.90 
14.45 

(Smirnoff.) 

64 
63 
62 

28.64 
28.17 
27.70 

53 
52 
51 

23.56 
23.11 
22.65 

32 
31 
30 

14.00 
13.56 
13.11 

+2H2O.    Sol.  inH2O. 
+3H2O.    Tr.  pt.  83°.    (Meyerhoffer,  Bull. 

61 
60 
59 
58 
57 
56 

27.24 
26.77 
26.30 
25.84 
25.38 
24.93 

50 
49 

48 
47 
46 

22.20 
21.74 
21.29 
20.83 
20.38 

29 
28 
27 
26 
25 

12.67 
12.23 
11.79 
11.35 
10.91 

oc.  1891  (3)  6,  85.) 
+4H2O.    Tr.  pt.  63°.    (Meyerhoffer.) 
+5H2O.     Very  deliquescent,  and  sol.  in 
[2O.    Decomp.  by  alcohol.    Sol.  in  HCl+Aq. 
Tr.  pt.  56°.    (Meyerhoffer.) 
+8H2O.    More  deliquescent  than  the  5H20 
alt.     Tr.  pt.  19°.    (Meyerhoffer.) 

(Heermann,  Ch.  Z.  1907,  31.  680.) 

+9H20     (Nollner,  Z.  Ch.  1865.  45.) 

1076 


TIN  HYDROGEN  CHLORIDE 


(6)  Metastannic  chloride. — Sol.  in  cold  H2O; 
solution  coagulates  on  boiling.  Cone.  HC1+ 
Aq  ppts.  from  SnQ4+Aq.  When  solution 
does  not  contain  HC1,  the  addition  of  HC1  + 
Aq  causes  a  ppt.,  which  dissolves  in  H5O. 
HNO3,  and  H2SO4+Aq  also  ppt.  K2SO4, 
Na2SO4,  and  NaCl+Aq  produce  ppts,.  insol. 
in  H2O,  but  sol.  in  HCl+Aq.  NH4C1  or 
KCl+Aq  do  not  ppt.  KNO3+Aq  ppts. 
slowly.  (Rose.) 

Tin    (stannous)    hydrogen   chloride,    SnCl2, 

HC1+3H20. 
Decomp.  by  H2O. 
Melts  at  -25°.     (Engel,  C.  R.  106.  1398.) 

Tin  (stannic)  hydrogen  chloride. 

See  Chlorostannic  acid. 

-  n 

Tin  (stannous)  hydrazine  chloride,  SnCl2, 
2N2H4,  HC1. 

Very  hydroscopic. 

Sol.  in  H2O  and  abs.  alcohol.  (Curtius.  J. 
pr.  1894,  (2)  60.  341.) 

Tin  (stannic)  chloride  with  MCI. 
See  Chlorostannate,  M. 

Tin  (stannous)  chloride  ammonia,  SnCl2, 
NH3. 

(Berzelius.) 

SnCl2,  4NH3.  Ppt.  (Naumann.  B.  1904, 
37.  4336.) 

Tin  (stannic)  chloride  ammonia,  SnCL, 
2NH3. 

Sol.  in  cold  H2O  without  decomp.,  but 
decomposes  by  heating. 

Tin  (stannous)  chloride  arsenate. 
See  Arsenate  chloride,  stannous. 

Tin  (stannic)  chloride  cyanhydric  acid.  SnCL, 
2HCN. 

Decomp.  on  moist  air  or  with  H2O.  (Klein. 
A.  74.  85.) 

Tin  (stannous)  chloride  hydrazine,  SnCl2 
2N2H4. 

Decomp.  by  H2O. 

Insol.  in  NH4OH+Aq.  (Franzen,  Z 
anorg.  1908,  60.  286.) 

Tin    (stannic)    chloride    nitrogen    sulphide 

SnCl4,  2N4S4. 

Insol.  in  most  solvents. 

Decomp.  by  warm  NH4OH+Aq. 

Decomposes  in  the  air.  (Wolbling,  Z 
anorg.  1908,  67.  284.) 

Decomp.  by  H2O.  (Davis,  Chem.  Soc 
1906,  89.  1576.) 


Tin    (stannic)    chloride   phosphine,    3SnCl4, 

2PH3. 
Decomp.  by  H2O.     (Rose,  Pogg.  24.  159.) 

Tin  (stannous)  chloride  potassium  stannous 

sulphate. 

See  Sulphate,  potassium  stannous  stannous 
chloride. 

Tin  (stannic)  chloride  sulphur  teZrachloride, 

SnCl4,  2SC14. 

Very  hygroscopic. 

Sol.  in  CHC13,  ligroin,  petroleum  ether, 
CS2,  POC13;  very  sol.  in  completely  dry 
absolute  ether,  in  benzene,  acetacetic  ester 
and  in  SC12.  (Ruff,  B.  1904,  37.  4517.) 

Tin  (stannic)  chloride  sulphide,  2SnCl4,  SnS2. 
See  Stannic  sulphochloride. 

Tin  (stannic)  chlorobromide,  SnClBr3. 

Decomp.  by  H2O.  (Ladenburg,  A.  suppl. 
8.  60.) 

SnCl2Br2.  Decomp.  by  H2O.  (Laden- 
burg.) 

Tin  (stannous)  chloroiodide,  SnClI. 

Decomp.  immediately  by  H2O.  (Henry, 
Phil.  Trans.  1845.  363.) 

Tin  (stannic)  chloroiodide,  SrCl2l2. 

Fumes  in  the  air. 

Decomp.  by  H2O.  (Lenormand,  J.  Pharm. 
1898.  8.) 

SnClIa.  (Lenormand,  J.  Pharm.  1899,  10. 
114.) 

Tin  (stannous)  fluoride,  SnF2. 

Easily  sol.  in  H2O.    (Berzelius,  Pogg.;  1.  34.) 

Tin  (stannic)  fluoride,  SnF4. 

Very  hydroscopic. 

Sol.  in  H2O.  Slowly  decomp.  in  aq.  solu- 
tion with  separation  of  Sn02.  (Ruff,  B.  1904, 
37.  681.) 

Tin  (stannic)  fluoride  with  MF. 
See  Fluostannate,  M. 

Tin  (stannous)  hydroxide,  2SnO,  H2O. 

Decomp.  to  SnO  when  boiled  with  H2O. 
More  easily  sol.  in  acids  than  Sn  or  SnO. 
Sol.  in  NaOH,  and  KOH+Aq,  even  when 
dil.  Insol.  or  very  si.  sol.  in  NH4OH, 
(NH4)2CO3,  and  K2CO3+Aq;  sol.  in  cold 
CaO2H2,  and  BaO2H2  with  decomposition 
on  boiling.  (Fremy,  A.  ch.  (3)  12.  460.)  Only 
si.  sol.  in  NH4Cl+Aq  hot  or  cold.  (Brett.) 
SI.  sol.  in  NaC2H3O2+Aq.  (Mercer.) 


TIN  IODIDE 


1077 


Solubility  in  NaOH+Aq. 


G.  Na  in  20  ccm. 

G.  Sn  in  20  ccm. 

0.2480 

0.3680 
0.6394 
0.8326 
0.9661 
2.1234 

0.1904 
0.2614 
0.4304 
0.5560     . 
0.7849 
1.8934 

(Rubenbauer,  Z.  anorg.  1002,  30.  335.) 

Not    pptd.    in    presence    of    Na    citrate. 

(Spiller.) 

Sol.  in  water-glass  +Aq.     (Ordway.) 
SnO2H2.     Solubility  in   1  1.  H2O  = 

0.0000135  g.  mol.  at  25°.     (Goldschmidt,  Z. 

phys.  Ch.  1906,  66.  389.) 

Tin  hydroxide,  SnO,  6SnO2+5H2O. 
+9H2O.     (Schiff,  A.  120.  153. 

Tin  sesg^uhydroxide,  Sn2O3,  xH2O. 

Insol.  in  H2O.  Sol.  in  NH4OH+Aq. 
(Fuchs,  J.  pr.  6.  318.) 

Tin  (stannic)  hydroxide. 

"a"  modification. 

Obtained  by  pptn.  by  alkali  in  stannic 
chloride  solution. 

Freshly  pptd.  substance  when  air  dried 
contains  73.5%  H2O;  when  dried  over  H2SO4 
or  in  a  vaccum  for  1  month  12.6%  H2O. 
Heated  to  glowing  loses  all  H2O  and  passes 
into  the  anhydride.  The  "a"  form  is  capable 
of  existing  in  all  degrees  of  hydration.  (Lorenz, 
Z.  anorg.  1895,  9.  372-375.) 

"a"  stannic  hydrate  is  a  white  amor- 
phous substance  which  is  very  sol.  in  HNO3 
when  moist;  sol.  in  H2SO4  even  dil.;  sol.  in 
HC1  and  not  pptd.  by  an  excess.  Very  sol. 
in  NaOH+Aq.  and  is  not  pptd.  by  an 
excess. 

A  solution  of  a  stannic  acid  in  HC1  is  iden- 
tical with  a  solution  of  freshly  prepared  aque- 
ous stannic  chloride  and  gives  no  ppt.  with  dil. 
HC1,  H2Sp4,  HNO3  or  arsenic  acid  even  on 
long  standing;. 

"  ft  "  modification. 

Obtained  by  oxiding  and  dissolving  Sn  hi 
HNO3,  and  from  solution  of  sodium  stannate 
by  pptn.  Freshly  pptd.  from  HNO3  when  air 
dried  contains  21.3%  H2O,  and  when  dried 
over  H2SO4  or  in  a  vacuum  11.3%,— corre- 
sponding to  Sn(OH)4  and  SnO  (OH)  2  respec- 
tively. 

Freshly  pptd.  from  sodium  stannate  solu- 
tion and  air  dried  contains  22.5%  H2O  and 
when  dried  over  H2SO4  or  in  a  vacuum  con- 
tains 12.1%,— corresponding  to  Sn(OH)4  and 
SnO  (OH)  2.  Passes  into  the  anhydride  when 
heated  to  glowing. 

The  "/3"  form  is  capable  of  existing  in  all 
degrees  of  hydration.  It  is  a  white  amor- 
phous substance  which  is  insol.  in  HN03;  in- 


sol in  H2SO4  even  when  cone.;  insol.  in  HC1 
changed  by  contact  with  the  acid  in 
;hat  when  the  acid  has  been  removed  the 
ppt.  is  readily  sol.  in  H2O,  though  pptd. 
again  from  solution  by  addition  of  HC1. 

hen  freshly  prepared  the  "ft"  form  is  sol. 
n  NaOH+Aq.  but  is  pptd.  by  an  excess  of 
NaOH. 

A  solution  of  "ft"  stannic  acid  in  HC1  be- 
haves quite  differently  from  an  aq.  solution 
of  stannic  chloride  in  that  it  ppts.  metas- 
tannic  sulphate  when  treated  with  H2SO4. 

This  ppt.  dissolves  when  heated  with  dilute 
HNO3  or  HC1,  but  the  solution  on  standing 
spontaneously  forms  another  ppt.  A  solution 
of  "ft"  stannic  acid  in  HC1  gives  a  ppt. 
when  treated  with  arsenic  acid.  (Lorenz, 
Z.  anorg.  1895,  9.  372.) 

See  also  Stannic  acid. 


Tin  hydroxyl  chloride,  SnO(OH)Cl. 
See  Chlorostannic  acid. 

Tin  (stannous)  iodide,  SnI2,  and  +2H2O. 

SI.  sol.  in  cold,  more  abundantly  in  hot 
H2O,  without  decomp. 

Solubility  in  H2O. 


t° 

Pts.  SnI2  in 
100  pts. 
solution 

t° 

Pts.  SnI2  in 
100  pts. 
solution 

98.5 

3.43 

97.3 

3.70 

84.9 

3.05 

87.4 

3.24 

73.9 

2.56 

77.6 

2.75 

60.1 

2.09 

67.5 

2.34 

51.5 

1.79 

59.7 

2.03 

41.0 

1.50 

49.5 

1.72 

30.5 

1.21 

39.4 

1.38 

20.8 

1.03 

29.6 

1.11 

19.8 

0.96 

(Young,  J.  Am.  Chem.  Soc.  1897,  19.  846.) 

Solubility  of  SnI2  in  HI+Aq  at  t°. 
Pts.  SnI2  per  100  pts.  solvent. 


t° 

20 
30 
40 
50 
60 
70 
80 
90 
100 

^M 

SSw 

^ 

S3 

0> 

£? 
o*-* 

^M 
2 

£? 

1s 

>§ 

SB 
X 

°s 
i 

iw 

0.98 
1.16 
1.40 
1.69 
2.07 
2.48 
2.95 
3.46 
4.03 

0.20 
0.23 
0.33 
0.46 
0.66 
0.91 
1.23 
1.65 
2.23 

0.60 
0.64 
0.71 
0.82 
1.11 
1.37 
1.83 
2.40 
3.63 

1.81 
1.81 
1.90 
2.12 
2.51 
2.92 
3.70 
4.58 
5.82 

4.20 
4.06 
4.12 
4.34 

4.78 
5.43 
6.38 

7.82 
9.60 

10.86 
10.28 
10.06 
10.35 
11.03 
11.97 
13.30 
15.52 

25.31 
23.46 
23.15 
23.76 
24.64 
25.72 
27.23 
•29.84 
34.05 

(Young,  J.  Am.  Chem.  Soc.fl897,  19.  851.) 


1078 


TIN  OXIDE 


Solubility  of  SnI2  at  low  temp,  in  29.95% 

Solubility  in  organic  solvents  at  t°. 

HI+Aq. 

G.  Snl4  in  100 

Sp   gr   of  the 

Temp. 

Pts.  in  100  pts. 
solution 

Pts.  in  100  pts. 
solvent 

Solvent 

t° 

g.  of  the  sat. 
solution 

sat.  solution 

1.5 
1.5 
6.0 
10.5 

12.96 
13.15 
12.35 
11.01 

14.89 

15.14 
14.09 
12.36 

CC14 
CC14 
CHC13 
C6H6 

22.4 
50.0 
28.0 
20.2 

5.25 
12.50 

8.21 
12.65 

1.59 
1.63 
1.50 
0.95 

15.2 

24.8 

10.48 
9.36 

11.70 
10.33 

(McDermott,  J.  Am.  Chem.  Soc.  1911,  33. 
1964) 

30.7 

8.78 

9.62 

04   o 

o  70 

9  50 

40  3 

9  51 

10.50 

Sol.   in    methyl    acetate.      (Naumann,   B. 

1909,  42.  3790.) 

(Young,  J.  Am.  Chem.  Soc.  1897,  19.  854.) 


Solubility  of  SnI2  at  low  temp,  in  39.6% 
HI+Aq. 


Temp. 

Pts.  in  100  pts.  of  solution 

Pts.  in  100  pts. 
of  solvent 

I 

II 

0° 
5.7° 
10.5° 
15.7° 
20.3° 

13.52 
16.44 
19.47 
23.56 
25.50 

13.56 
16.37 
19.60 
23.68 
25.60 

15.66 
19.71 
24.27 
30.92 
34.30 

(Young,  J.  Am.  Chem.  Soc.  1897,  19.  852- 
853.) 


Sol.  in  SnCl2+Aq.  Sol.  in  warm  alkali 
chlorides  or  iodides  +  Aq;  also  in  dil.  HC1+ 
Aq.  Very  si.  sol.  in  CHC13,  CS2,  or  C6H6. 
(Personne,  C.  R.  54.  216.) 

Sol.inKOH+Aq.  (Rose.) 

Sol.  in  acetone.  (Naumann,  B.  1904,  -37. 
4328.) 


Tin  (stannic)  iodide,  SnI4. 

Decomp.  by  H2O  into  SnO2  and  HI. 

Very  sol.  in  PC13.  (Beckmann,  Z.  anorg. 
1906,  51.  110.) 

Sol.  in  POC13,  (Walden,  Z.  anorg.  1900, 
25.212.). 

Easily  sol.  in  PC13  and  PBr3.  (Walden, 
Z.  anorg.  1900,  25.  211.) 

Sol.  in  liquid  AsBr3  forming  a  solution 
with  sp.  gr.  =3.731  at  1£°.  (Retgers,  Z. 
phys.  Ch.  1893,  11.  342.) 

Sol.  in  SOC12,  S2C12  and  SO2C12.  (Walden, 
Z.  anorg.  1900,  26.  215.) 

Sol.  in  SnCl4.     (Walden.) 

Sol.  in  anhydrous  alcohol,  ether,  and 
benzene.  1  pt.  CS2  dissolves  .1.45  pts.  SnI4 
at  ordinary  temp.  (Schneider,  Pogg.  127. 
624.) 

100  pts.  methylene  iodide,  CH2I2f  dissolve 
22.9-  pts-.  -Sftlr  a4- 10°-.— -Sfh- gr^-ef  solution  = 
3.481.  (Retgers,  Z.  anorg.  3.  343.) 


(Eidman,   C.   C.   1899, 


'Ut7,     ' 

Sol.   in   acetone. 
II.  1014.) 

Solubility  in  CS2. 

100  g.  of  the  sat.  solution  contain  at: 
—  58°    —84°    —89°    —94°    —114.5° 
16.27     10.22       9.68     10.65        9.41  g.  SnI4. 
(Arctowski,  Z.  anorg.  1896,  11.  274.) 


Sol.  in  allyl  mustard  oil. 
phys:  Ch.  1905,  9.  647.) 


(Mathews,  J. 


Tin  (stannous)  hydrogen  iodide,  SnI2,  HI. 

Not  obtained  in  pure-  state.  (Young,  J. 
Am.  Chem.  Soc.  1897, 19.  856.) 

Tin  (stannous)  iodide  ammonia)  SnI2,  2NH3. 
(Ephraim  and  Schmidt,  B.  1909,  42.  3857.) 
SnI4,  8NH3.  (Ephraim  and  Schmidt.) 

Tin  (stannic)  iodide  ammonia,  SnI4,  3NH3. 

(Personne,  C.  R.  54.  218:) 

SnI4,  4NH3.     (Personne.) 

SnI4,  8NH3.  (Rammelsberg,  Pogg.  48. 
169.) 

Tin  iodosulphide, 
See  Tin  sulphoidide. 

Tin  monoxide  (Stannous  oxide),  SnO. 

Insol.  in  H2O.  Sol.  in  acids.  Very  si.  sol. 
in  boiling  NH4Cl+Aq.  (Rose.)  Insol.  in 
NaOH  or  KOH+Aq. 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  830.) 

Insol.  in  acetone.  (Naumann,  B.  1904,  37. 
4329.) 

Tin  dioxide  (Stannic  oxide),  SnO2. 

Insol.  in  H2O  or  cone,  acids  except  cone 
H2SO4.  Insol.  in  cone,  alkalies  or  NH4OH+ 
Aq. 

Not  absolutely  insol.  in  dil.  HNO3+Aq. 
(Mulder.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  830.) 

Mia.  Cassiterite  (Tin  ^tone).  Not  attacked 
by  acids. 


TIN  SULPHIDE 


1079 


Tin  sesquioxide,  Sn2O3. 

While  moist,  easily  sol.  in  NH4OH+Aq. 
SI.  sol.  in  dil.,  more  easily  in  cone.  HCl+Aq. 

(Berzelius.) 

Tin  (stannic)  oxybromide,  Sn3Br6O  +  12H2O. 

Decomp.  by  H2O  into  SnBr2  and  H2SnO3. 

Sn3Br8O2.  As  above.  (Preis  and  Ray- 
mann,  C.  C.  1882.  773.) 

Tin    (stannic)    oxybromide    nitrogen    pent- 
oxide,  SnO2,  3Br2,  N2O6. 
Decomp.  by  H2O.     (Thomas,  C.  R.  1896, 
122.  33.) 

Tin  (stannous)  oxychloride,  SnO,  SnCl2+ 
3H2O. 

Insol.  in  H2O.  Sol.  in  HC1,  HC2H3O2,  and 
dil.  HNO3,  or  H2SO4+Aq.  (J.  Davy,  Schw. 
J.  10.  325.) 

Sn8Cli4O8  +  10H2O.  Easily  sol.  in  H2O  or 
alcohol. 

Can  be  recrystallized  from  alcohol  but 
not  from  H2O.  (Tschermak,  W.  A.  B.  44. 
2.  736.) 

3SnO2,  2SnCl2+6H2O.  Very  si.  sol.  in 
H2O.  Sol.  in  dil.  acids.  (Ditte,  A.  ch.  1882, 
(5)  27.  146.) 

4SnO,  SnCl2+6H2O.  (Ditte.) 

Tin  (stannic)  oxychloride,  SnO2,  SnCl4. 
Sol.   in  H2O.      (Scheurer-Kestner,   A.   ch. 

(3)  47.  6.) ' 

Tin  (raetostannic)  oxychloride,  3SnO2,  SnCl4 
+3H2O. 

Sol.    in    little,    decomp.    by    much    H2O. 
(Weber,  Pogg.  122.368.) 
4SnO2,  SnCl4+7H2O.     (Weber.) 

"Metastannyl  chloride  ft,"  Sn6O9Cl2.  De- 
liquescent. Sol.  without  decomp.  in  a  small 
amount  of  H2O  or  in  a  large  amount  of  H2O 
containing  a  few  drops  HC1. 

Sol.,  in  abs.  alcohol.  (Engel,  C.  R.  1897, 
124.  767.) 

+4H2O  and  +9H2O.  Sol.  in  H2O  acidified 
with  one  drop  of  HC1.  Pptd.  by  excess  HC1. 
(Engel,  C.  R.  1897,  124.  768.) 

"Pamstannyl  chloride,"  Sn6O9Cl2+2H20. 
Decomp.  by  excess  H2O. 

Sol.  in  H2O;  pptd.  by  HC1.  (Engel,  C.  R. 
1897,  126.  465.) 

Tin  (stannic)  oxychloride  nitrogen  pent- 
oxide,  SnOCl2,  3SnCl4,  N2O6. 

Hydroscopic;  sol.  in  H2O. 

Decomp.  by  heat.  (Thomas,  C.  R.  1896, 
122.  32.) 

Tin     (stannous)     oxyiodide,     SnO,     3SnI2 
2SnO,  3SnI2;  SnO,  SnI2;  and  2SnO,  SnI2 
.    Decomp.  by  much  H2O.      (Personne,  C.  R 
54.  216.) 


Tin  oxysulphide,  Sn2S3O+llH20. 

Very  sol.  in  (NH4)2CO3+Aq;  slowly  sol. 
n  H20.  (Schmidt,  B.  1894,  27.  2739.) 

Tin  phosphide,  Sn2P. 

(Ragg,  C.  C.  1898,  II.  170.) 

SnP.  Sol.  in  HCl+Aq.  Insol.  in  HNO3 
+Aq. 

SnP2.  Not  attacked  by  HC1.  Easily  at- 
tacked by  aqua  regia.  (Emmerling,  B.  1879. 
12.  155.) 

SnP3.  Insol.  in  HC1.  Slowly  attacked  by 
dil.  HNO3  at  50°.  Oxidized  by  fuming  HNO> 
with  ignition.  (Jolibois,  C.  R.  1909,  148. 
638.) 

Sn3P2.    Insol.  in  mercury. 

Decomp.  by  HC1.  (Stead,  J.  Soc.  Chem. 
Ind.  1897,  16.  206.) 

Sn4P3.  Attacked  by  HC1,  HNO3  and  al- 
kalies. (Jobilois,  C.  R.  1909,  148.  637.) 

The  only  true  compounds  are  Sn4P3  and 
SnP3.  (Jolibois,  C.  R.  1909,  148.  637.) 

Tin  phosphochloride,  Sn3P2Cl«. 
(Mahn,  Jena.  Zeit.  5.  1660.) 

Tin  (stannous)  selenide,  SnSe. 

Decomp.  by  boiling  HCl+Aq.  Slowly 
oxidised  by  boiling  HNO3+Aq,  and  easily 
dissolved  in  aqua  regia  (Schneider,  Pogg. 
127.  624.)  Easily  sol.  in  alkalies +Aq 
(Uelsmann,  A.  116.  122),  or  scarcely  even  on 
boiling  (Schneider),  according  to  method 
of  preparation.  Sol.  in  alkali  sulphides  or 
selenides  +Aq. 

Tin  (stannic)  selenide,  SnSe2. 

Not  attacked  by  H2O  or  dil.  acids;  scarcely 
attacked  by  boiling  cone.  HCl+Aq;  gradu- 
ally decomp.  by  hot  HNO3+Aq;  easily  dis- 
solved by  warm  aqua  regia,  and  hot  cone. 
H2S04. 

Sol.  in  cold,  more  easily  in  warm  KOH, 
NaOH,  or  NH4OH+Aq.  (Uelsmann,  A. 
116.  122.) 

Tin  (stannous)  sulphide,  SnS. 

1  1.  H2O  dissolves  0.14X10-6  mols.  SnS 
at  18°.  (Weigel,  Z.  phys.  Ch.  1907,  68.  294.) 

Insol.  in  dil.,  sol.  in  cone.  HCl+Aq.  SI. 
sol.  in  hot  cone.  HNO3+Aq.  Insol.  in  KOH 
+Aq. 

+H2O.  Insol.  in  H2O,  H2S+Aq,  or  dil. 
acids;  sol.  with  decomp.  in  cone,  acids; 
easily  sol.  in  hot  cone.  HCl+Aq.  Insol. 
in  H2SO3+Aq.  Insol.  in  NH4OH+Aq. 
Insol.  in  NH4C1,  or  NH4NO3+Aq.  Scarcely 
sol.  in  (NH4)2S+Aq,  but  easily  sol.  in  the 
same  on  addition  of  S.  (Rose.) 

10%  NaOH+Aq  dissolves  SnS  by  violent 
boiling. 

Insol.  in  cold,  si.  sol.  in  hot  Na2SO3+Aq. 
(Materne,  C.  C.  1906,  II.  557.) 

Sol.  in  alkali  polysulphides+Aq. 

Insol.  in  acetone.     (Eidmann,  C.  C.  1899, 


1080 


TIN  SULPHIDE 


II.   1014);   (Naumann,  B.   1904,  37.  4329.); 
ethyl  acetate.    (Naumann,  B.  1910,  43.  314.) 

Tin  (stannic)  sulphide,  SnS2. 

Anhydrous.  (Mosaic  gold.)  Insol.  in  HC1 
or  HNO3+Aq,  but  decomp.  by  aqua  regia. 
Sol.  in  hot  KOH+Aq  or  K2CO3+Aq;  also 
in  hot  K2S,  Na2S+Aq,  and  (NH4)2S+Aq. 

1  1.  H2O  dissolves  1.13X10-6  mols.  SnS2 
at  18°.  (Weigel,  Z.  phys.  Ch.  1907,  58.  294.) 

+zH2O.  SI.  sol.  in  NH4OH+Aq,  but 
readily  in  KOH,  KssS,  or  Na2S+Aq;  also  in 
hot  cone.  HCl+Aq.  Decomp.  by  hot  HNO3 
+Aq.  Insol.  in  KHSOa+Aq.  Sol.  in  K2GO3 
+Aq.  Insol.  in  NH4C1,  and  NH4NO3+Aq. 
(Brett.) 

Pptd.  SnS2  is  insol.  in  cold,  sol.  in  hot 
Na2B4O7  +Aq.  Sol.  in  Na2CO3+Aq.  Very 
sol.  in  NaOH+Aq.  (Materne,  C.  C.  1906, 

II.  557.) 

Sol.  in  boiling  cone.  H2C2O4+Aq.  (Clarke, 
C.  N.  21.  124.) 

Insol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  -3790);  ethyl  acetate  (Naumann, 

B.  1910,  43.  314.);  acetone    (Naumann,  B. 
1904,   37.   4329;  Eidmann,  C.  C.  1899,   II. 
1014.) 

Tin  sesg-w'sulphide,  Sn2S3. 

Sol.  in  moderately  cone.  HC1.  (Antony 
and  Niccoli,  Gazz.  eh.  it.  1892,  22.  (2)  408.) 

Tin  sulphochloride,  SnS2,  2SnCl4. 

H2O  dissolves  out  SnCl4.  (Dumas,  Schw. 
J.  66.  409.) 

SnS2Cli2  =  SnCl4,  2SC14.  Sol.  in  H2O  with 
separation  of  S. 

Gradually  sol.  in  dil.  HNO3+Aq. 

Sol.  in  POC13.     (Casselmann,  A.  83.  267.) 

Tin  sulphoiodide,  SnS2l4. 

Decomp.  by  H2O  into  SnO2,  S,  and  HI; 
by  cold  cone.  HCl+Aq  with  separation  of  S, 
also  by  aqua  regia,  and  HNO3+Aq. 

Cold  KOH+Aq  separates  S  and  SnO2. 

Completely  sol.  in  hot  KOH+Aq. 

Sol.  in  cold,  more  easily  in  hot  CS2  or 
CHC13. 

Decomp.   by   alcohol.      (Schneider,    Fogg. 

III.  249.) 

Tin   sulphophosphide,   Sn3P2S. 

Insol.  in  HC1,  HNO3  and  aqua  regia. 

Sol.  in  aq.  alkali  hydroxides,  containing 
C12  or  Br2  in  solution.  (Granger,  C.  R.  1896, 
122.  322.) 

Tin  (stannous)  telluride,  SnTe. 

Not  attacked  by  cone.  HCl+Aq.     (Ditte, 

C.  R.  97.  42.) 

Titanic  acid,  TiO2,  xH2O. 

a-Titanic  add. — Insol.  in  H2O  or  alcohol. 
When  dried  in  the  cold,  is  completely  sol.  in 


acids,  especially  HC1,  or  dil.  H2SO4+Aq,  but 
when  the  solution  in  acids  is  boiled,  it  is  con- 
verted into  /3- titanic  acid.  Very  si.  sol.  even 
when  moist  in  H2SO3+Aq.  (Berthier.)  SI. 
sol.  in  alkali  carbonates  +Aq.  A  complete 
solution  in  an  alkali  carbonate  +Aq  can  only 
be  obtained  by  adding  a  Ti  salt  drop  by  drop 
to  the  alkaline  solution,  and  allowing  the 
ppt.  to  dissolve  entirely  before  adding  more 
Ti  salt.  On  boiling  the  solution  in  (NH4)2CO3 
+Aq  (or  in  K2CO3  or  NaaCO3+Aq  with 
NH4C1)  the  titanic  acid  is  pptd. 

Relatively  easily  sol.  in  mineral  acids,  de- 
creasing in  the  following  order  HC1,  HNO3, 
H2SO4.  Insol.  in  perchloric  acid.  (Lan- 
decker,  Z.  anorg.  1909,  64.  67.) 

Sol.  in  dil.  H2SO4.  40  g.  H2O  +  70  g. 
H2SO4  (sp.  gr.  1.145)  dissolves  0.33  g.  TiO2 
in  15  min.  (Hall  and  Smith,  Proc.  Am. 
Phil.  Soc.  1905,  44.  193.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  830.) 

p-Titanic  acid,  Metatitanic  acid. — Insol. 
in  H2O,  acids  except  HF,  or  alkali  hydrates  or 
carbonates  +Aq.  When  digested  with  cone. 
H2SO4  until  acid  is  evaporated,  the  residue 
is  sol.  in  H2O.  (Berzelius.) 

y-Titanic  acid. — Sol.  in  pure  H2O,  but 
/3-acid  is  pptd.  by  boiling.  (Knop,  A.  123 
351.) 

Colloidal  TiO2  :rH2O+Aq  has  been  pre- 
pared by  Graham  (Chem.  Soc.  17.  325.) 

Barium  titanate,  2BaO,  3TiO2. 
(Bourgeois,  C.  R.  103.  141.) 

Barium  pertitanate  peroxide. 
See  Pertitanate,  barium  peroxide. 

Calcium  titanate,  CaTiO8. 

(Ebelmen,  C.  R.  32.  711.) 

Min.  Perofskite.  Scarcely  attacked  by 
HC1  +Aq  or  other  acids,  except  hot  H2SO4, 
which  decomposes  it. 

CaO,  2TiO2.  Min.  Tilanomorphite.  Par- 
tially decomp.  by  HCl+Aq,  completely  by 
H2SO4. 

Cobaltous  titanate,  CoTi03. 
(Bourgeois,  C.  C.  1893,  I.  226.) 

Ferrous  ortfotitanate,  Fe2TiO4. 
(Hautefeuille,  C.  R.  69.  733.) 

Ferroferric  titanate,  FeTiO3,  zFe2O3. 

Min.  Menaccanite.  Very  si.  sol.  in  HC1  or 
aqua  regia  with  separation  of  TiO2. 

Ferric  titanate. 

Not  attacked  by  boiling  H2SO4  or  cone. 
HCl+Aq.  (Wohler  and  Liebig,  Pogg.  21. 
578.) 


TITANIUM  CHLORIDE 


1081 


Magnesium  titanate,  MgTiO3. 

Insol.  in  H2O  and  acids.  (Hautefeuille,  A. 
ch.  (4)  4.  169.) 

Min.     Geikielile. 

When  finely  powdered,  is  easily  sol.  in  hot 
HC1,  or  in  cold  HF  in  a  few  hours.  (Dick, 
Miner,  Mag.  1894,  10.  146.) 

Mg2TiO4.  Slowly  decomp.  by  boiling 
with  HNO3+Aq.  (Hautefeuille,  A.  ch.  (4) 
4.  169.) 

Potassium  titanate,  K2TiO|. 

Anhydrous.    Decomp.  with  H2O. 

+4H2O.  Deliquescent.  Very  sol.  in  H2O. 
Precipitated  from  aqueous  solution  by  alcohol. 
(Demoly,  Compt.  chim.  1849.  325.) 

Potassium  titanate,  acid,  K2O,  3TiO2  +2H2O 

Insol.  in  H2O.     (Demoly.) 

K2O,  6TiO2+2H2O.     (Demoly.) 

K2O,  3TiO2+3H2O.  Insol.  in  H2O.  Com- 
pletely sol.  in  HCl+Aq  if  only  cold  H2O  is 
used  for  washing.  When  heated  to  100°,  no 
longer  completely  sol.  in  HCl+Aq.  (Rose, 
Fogg.  74.  563.) 

K2O,  12TiO2.     (Rose,  Gilb.  Ann.  73.  78.) 

Sodium  titanate,  Na2TiO3. 

Anhydrous.  Decomp.  by  H2O  into  NaOH, 
and  an  acid  titanate,  insol.  in  H2O. 

+4H2O.  Deliquescent.  Very  sol.  in  H2O. 
Precipitated  from  aqueous  solution  by  alcohol 
(Demoly.) 

Sodium  titanate,  acid,  2Na2O,  9TiO2+5H2O 

If  not  heated  to  100°,  is  sol.  in  cold  HC1+ 
Aq.  (Rose,  Gilb.  Ann.  73.  78.) 

2Na2O,  3TiO2.  Insol.  in  H2O;  slowly  sol 
in  cold,  easily  in  hot  HCl+Aq.  (Cormim- 
bceuf,  C.  R.  115.  823.) 

Na2O,  2TiO2.    As  above.     (C.) 

Na2O,  3TiO2.  Insol.  in  H2O,  and  nearly 
so  in  boiling  HCl+Aq.  (C.) 

Strontium  titanate,  2SrO,  3TiO2. 
(Bourgeois,  C.  R.  103.  141.) 

Zinc  titanate,  ZnO,  TiO2(?). 

(Uvy,  A.  ch.  (6)  24.  456.) 

2ZnO,  TiO2(?).    '(L4vy.) 

3ZnO,  2TiO2.  Slowly  attacked  by  warn 
H2SO4  or  HNO3+Aq,  and  by  H2SO4+HF 
Wholly  sol.  in  cold  HCl+Aq.  (Le"vy.) 

-  4ZnO,  5TiO2.  Not  attacked  by  cold  cone 
acids,  but  sol.  by  boiling  except  in  HCl+Aq 
(Levy.) 

ZnO,  3TiO2.  Insol.  in  H2O,  alcohol,  o 
ether.  Dil.  HNO3,  H?SO4,  or  HCl+Aq  do 
not  attack  even  on  boiling;  boiling  H2SO4  dis 
solves  with  difficulty;  not  attacked  by  cone 
boiling  alkalies +Aq.  (L6vy,  A.  ch.  (6)  26 
471.) 

Pertitanic  acid. 
See  Pertitanic  acid. 


Itanium,  Ti. 

Decomp.  H2O  even  under  100°  (Wohler); 
lot  attacked  by  H2O  under  500°.  (Kern,  C.  N. 
3.  57). 

Does  not  decomp.  H2O  at  100°. 
Schneider,  Z.  anorg.  1894,  8.  85.) 

Sol.  in  HCl+Aq  if  warmed.  Rapiclly  sol. 
n  HF+Aq.  Sol.  in  cold  dil.  H2SO4+Aq, 
HNO3+Aq,  or  HC2H3O2+Aq.  Dissolves 
almost  instantaneously  in  HF+Aq.  (Merz.) 

Sol.  in  molten  lead  and  iron;  sol.  in  HC1, 
HNO3  and  aqua  regia.  (Moissan,  C.  R.  1895, 
120.  293.) 

Amorphous.  Loses  its  spontaneous  in- 
lammability  when  left  for  a  time  in  contact 
with  H2O.  (Schneider,  Z.  anorg.  1895,  8.  85.) 

Titanium  amide,  Ti(NH2)4. 

Violently  attacked  by  H2O.  (Stahler,  B. 
1905,  38.  2629.) 

Titanium  fribromide,  TiBr3+6H2O. 

Very  hydroscopic.  (Stahler,  B.  1904,  37. 
4409.) 

Titanium  teJrabromide,  TiBr4. 

Deliquescent.  Decomp.  by  H2O.  (Duppa, 
R.  42.  352.) 

Sol.  in  absolute  alcohol  and  in  dry  ether. 
(Rosenheim  and  Schiitte,  Z.  anorg.  1900, 
24.  238.) 

Titanium  bromonitride,  TiNBr. 

Decomp.  by  a  small  amount  of  H2O.  On 
addition  of  more  H2O,  a  part  dissolves  form- 
ing a  solution  which  decomp.  on  warming 
with  separation  of  titanic  acid.  It  behaves 
similarly  toward  dil.  HNO3,  dil.  HC1  and  dil. 
H2SO4.  Completely  sol.  in  warm  dil.  H2SO4. 
(Ruff,  B.  1908,  41.  2262.) 

Titanium  carbide,  TiC. 

Sol.  in  HNO3+Aq.  (Shinier,  C.  N.  66.  71.) 
Insol.  in  HC1.  Slowly  sol.  in  aqua  regia. 

(Moissan,  C.  R.  1895,  120.  295.) 

Titanium  carbide  nitride,  Ti10C2N8 =Ti(CN)2, 

3Ti3N2. 

Insol.  in,  and  not  attacked  by  boiling  HNOS 
or  H2SO4  (Wollaston),  but  sol.  in  HNO3+HF 
(Berzelius) . 

Titanium  bichloride,  TiCl2. 

Very  deliquescent.  Decomposes  H2O  with 
violence.  Insol.  in  ether,  CS2,  or  CHC13. 
Decomp.  by  99.5%  alcohol. 

Titanium  trichloride,  TiCl8. 

Deliquescent.  Sol.  in  H2O  with  evolution 
of  heat. 

+4H2O.    (Glatzel,  B.  9.  1829.) 

+6H2O.  Very  sol.  in  H2O.  (Polidori,  Z. 
anorg.  1898,  19/307.) 


1082 


TITANIUM  CHLORIDE 


Titanium  tefrachloride,  TiCl4. 

Anhydrous.  Sol.  in  H2O  with  evolution  of 
much  heat. 

+5H2O.     Deliquescent. 

Titanium  sulphuryl  chloride,  TiCl4SO3  = 

TiCl3OSO2Cl. 

Deliquesces  gradually  in  moist  air.  (Claus- 
nitzer,  B.  11.  2011.) 

Titanium  chloride  ammonia,  TiCl4,  4NH3. 

Deliquescent.  Solution  in  H2O  is  not 
quite  clear.  (Rose.) 

According  to  Persoz  (A.  ch.  46.  315),  is 
TiCU,  6NH3. 

TiCl4,  6NH3  and  TiCl4,  4NH3. 

Both  compds.  are  unstable  in  moist  air; 
insol.  in  ether.  (Rosenheim,  Z.  ahorg.  1901, 
26.  245.) 

TiCl4,  8NH3.  Violently  decomp.  by  H2O. 
(Stabler,  B.  1905,  38.  2627.) 

Titanium  te/rachloride  cyanobromide, 

TiCl3,  NCClBr. 
(Schneider,  Z.  anorg.  1894,  8.  92.) 

Titanium  chloride  cyanhydric  acid,  TiCl4, 
2HCN. 

Deliquescent.  Sol.  in  H2O  with  evolution 
of  heat.  (Woliler,  A.  73.  226.) 

Titanium  bichloride  nitrogen  sulphide. 

2TiCl3,  N4S4. 

Decomp.  rapidly  in  air.  (Davis,  Chem. 
Soc.  1906,  89.  (2)  1576.) 

Titanium  te^rachloride  nitrogen  sulphide, 
TiCl4,  N4S4. 

Hydroscopic. 

Decomp.  by  H2O,  HNO3,  HC1,  KO&  and 
alcohol.  (Wolbling,  Z.  anorg.  1908,  57.  282.) 

Titanium  chloride  phosphine. 

Decomp.  by  H2O,  HCl+Aq,  KOH+Aq, 
K2CO3+Aq,  or  (NH4)2CO3+Aq.  (Rose.) 

Titanium   trichloride   phosphoryl  chloride, 

TiCl4,  2POC13. 
'(Ruff,  B.  1903,36.  1783.) 

Titanium  chloronitridej  TiNCl. 

Decomp.  by  small  amount  cold  H2O.  On 
the  addition  of  more  H2O  it  is  only  partially 
decomp.  v  For  complete  solution,  the  addition 
of  dil.  HC1  or  a  mixture  of  warm  dil.  H2SO4 1 
and  HF  is  necessary.  Easily  sol.  in  cone. 
HNO3  and  in  cone.  H2SO4.  (Ruff,  B.  1908, 
41.  2259.) 

Titanium  cfofluoride. 
.    (Hautefeuille,  C.  R.  67.  151.) 
Probably  sesquiftuoride. 


Titanium  ses<?iufluoride,  Ti2F6. 

Appears  to  be  two  modifications,  one  soL 
in  H2O,  and  the  other  insol.  in  H2O.  (Haute- 
feuille, C.  R.  69.  189.) 

Insol.  in  H2O.     (Weber,  Pogg.  120.  292.) 

Titanium  te^rafluoride,  TiF4. 

Decomp.  by  H2O.    (Unverdorben.) 

Sol.  in  H2O,  but  solution  decomp.  upon 
evaporation.  (Marignac,  Ann.  Min.  (5)  15. 
258.) 

Sol.  in  H2O.     (Emich,  M.  1904,  25.  910.) 

Very  hydroscopic. 

Sol.  in  H2O.  -  SI.  sol.,  in  cone.  HF+Aq. 

Sol.  in  cold  POC13  without  decomp.  De- 
comp. in  warm  POC13. 

Sol.  in  alcohol  and  dry  pyridine. 

Insol.  in  ether,  CS2,  CC14,  SiCl4,  SiBr4, 
S02C12,  SOC12,  SCI,,  AsCl3,  S03,  CrO3,  PCI,. 
(Ruff,  B.  1903.  36.  1780.) 

+2H2O.  Sol.  in  H2O.  (Ruff,  B.  1903,  36. 
1780.) 

Titanium  hydrogen  fluoride,   2HF,    TiF4  = 

H2TiF6. 

Sol.  in  H2O  with  decomposition  and  separa- 
tion of  a  basic  salt.  Corresponds  to  fluosilicic 
acid,  and  may  be  considered  as  fluotitanic 
acid  H2TiF6. 

Titanium  fluoride  with  MF. 
See  Fluotitanate,   M. 

Titanium  teZrafluoride  ammonia,  TiF4;  2NH3. 
Sol.  in  H2O;  decomp.  in  aq.  solution  on 
boiling.    (Ruff,  B.  1903,  36.  1781.) 

Titanium  wo7?ohydroxide,  TiO2H2. 
Ppt.    (Wohler,  A.  73.  49.) 
.  Ti3O4H.    Not  attacked  by  cold  cone,  acids; 
si.  attacked  on  warming.     Insol.  in  cold  or 
hot  KOH+Aq.    (Winkler,  B.  1890,  23.  2659.) 

Titanium  segmhydroxide,  Ti2O3,  zH2O. 

Decomposes  very  quickly  with  H2O,  form- 
ing titanium  efahydroxide. 

TiO3H3.    (Polidori,  Z.  anorg.  1899, 19. 306.) 

Titanium  ^"hydroxide. 
See  Titanic  acid. 

Titanium   hydroxychloride,    TiCl3(OH). 

Deliquescent.  Easily  sol.  in  H2O  and  al- 
cohol. Sol.  in  ether. 

TiCl2(OH)2+lHH2O.  .Deliquescent.  Sol. 
in  H2O,  alcohol,  and  ether.  Aqueous  solution 
decomp.  by  boiling. 

TiCl(OH)3+H2O.  Nearly  insol.  in  H2O. 
Insol.  in  alcohol  and  ether.  (Konig  and  v. 
der  Pfordteuj-  B.  21.  1708.) 

See  alsor  Titanium  oxychloride. 

Titanium  diiodide,  TiI2. 

Very  hydroscopic;  insol.  in  organic  solvents; 
sol.  in  cone.  HF  and  boiling  HC1;  deeomp.  by 


TITANOMOLYBDIC  ACID 


1083 


H2O,  alkalies,  H2SO4  and  HNO3.     (Defacqz, 
C.  R,  1908,  147.  66.) 

Titanium  ^iodide,  TiI3+6H2O. 

Very  hydroscopic.  (Stabler,  B.  1904,  37. 
4410.) 

Titanium    tefraiodide,    TiI4. 

Fumes'on  air,  and  dissolves  rapidly  in  H2O 
with  evolution  of  heat.  Solution  decomposes 
on  standing.  (Weber.) 

Titanium  nitride,  Ti3N4. 

Difficultly  sol.  in  warm  HNO3-f-Aq.  More 
easily  sol.  in  aqua  regia.  (Rose.) 

Insol.  in  dil.  acids.  Decomp.  by  hot  cone. 
H2Sp4  and  by  cone.  HNO3,  especially  when 
HF  is  added,  and  by  boiling  KOH+Aq. 
(Ruff  and  Eisner,  B.  1908,  41.  2252.) 

Decomp.  by  H2O  and  dil.  acids. 

Insol.  in  all  ordinary  indifferent  organic 
solvents.  (Ruff,  B.  1912,  45.  1369.) 

TiN2.    Insol.  in  H2O.     (Wohler.) 

Is  TiN,  according  to  Guerin  (C.  R.  82.  972.) 

Titanium  monoxide,  TiO. 

(Moissan,  C.  R.  1895,  120.  290.) 

Titanium  sesgwoxide,  Ti2O3. 

Insol.  in  HC1  or  HNO3+Aq.  Difficultly 
sol.  in  H2SO4.  (Ebelmen,  A.  ch.  (3)  20.  392.; 

When  moist,  insol.  in  H2O  or  NH4OH+Aq 
but  quickly  decomp.  to  TiO2.  Sol.  in  oxygen 
acids,  but  quickly  decomp.  (Berzelius.)- 

Titanium  dioxide,  TiO2. 

Amorphous.  Insol.  in  H2O,  HC1,  or  dil 
H2SO4+Aq,  even  when  heated  for  a  long 
time. 

Sol.  in  cone.  H2SO4  by  long  digestion. 

TiO2,  strongly  ignited  at  1000°,  is  practi 
cally  insol.  in  cone.  H2SC>4  and  HF. 

When  less  strongly  ignited  (by  heating 
ortho  or  metatitanic  acid  to  700°)  it  is  easily 
sol  therein.  (Bornemann  and  Schirrmeister 
C.  C.  1910,  II.  1870.) 

Ignited  TiO2  is  very  difficultly  sol.  in  HF 
(Pennington,  J.  Am.  Chem.  Soc.  1896,  18 
56  ) 

The  solubility  of  ignited  TiO2  in  H2SO 
is  helped  by  H2O2.  (Weiss  and  Landecker 
Z.anorg.  1909,64.71.) 

The  solubility  in  H2SO4  is  increased 
addition  of  H2O2.  H2O2  brings  TiO2  quickly 
and  completely  into  solution  in  the  presenc 
of  NH4OH,  NH4C1,  NaOH,  Na2CO3  am 
Na2HPO4.  (Weiss  and  Landecker,  m  anorg 
1909,64.71.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  , 
1898,  20.  830.) 

Crystalline.  Min.  Rutile,  Brookite,  an 
Anatase.  Solubility  as  above. 

See  also  Titanic  acid. 


itanium  oxide,  Ti3O5. 

(Deville,  C.  R.  53.  163.) 

True  formula  is  Ti7O]2.  (v.  der  Pfordten, 
L  237.  201.) 

Titanium   peroxide,   TiO3. 

Sol.  in  acids.  Solution  in  H2SO4  is  very 
table,  but  the  HC1  solution  decomposes  very 
asily.  (Weber,  B.  16.  2599;  Piccini,  B.  15. 
!221;  Classen,  B.  21.  370.) 

Titanium  oxychloride,  TiO2,  TiOCl2+8H2O. 

Sol.  in  much  H2O.  (Merz,  Bull.  Soc.  1867. 
401.) 

Ti2O2Cl2.  Insol.  in  H2O.  Sol.  in  NH4OH  + 
A.q  with  separation  of  TiO2. 

See  also  Titanium  hydroxychloride. 

Titanium  oxyfluoride. 

Insol.  in  H2O.    (Berzelius.) 

Titanium  oxyfluoride  with  MF. 
See  Fluoxypertitanate,  M. 

Titanium  phosphide,  TiP. 

SI.  sol.  in  boiling  aqua  regia. 
Insol.  in  dil.  or  cone,  acids  and  alkalies. 
SI.  attacked  by  fuming  HNO3  in  sealed 
tube  at  250°-3006.     (Gewecke,  A.  1908,  361. 

84.) 

Titanium  phosphochloride. 

See  Phosphorus  titanium  chloride. 

Titanium  silicide,  TiSi2. 

Sol.  in  HF;  insol.  in  other  n?in.  acids. 

Slowly  sol.  in  10%  KOH+Aq.  (Honig- 
schmid,  C.  R,  1906,  143.  226.) 

Titanium  wonosulphide,  TiS. 

Insol.  in  alkalies.  Difficultly  sol.  in  nitric 
acid  and  aqua  regia. 

Insol.  in  HF.     (v.  der  Pfordten,  A.  234. 

257.) 

Titanium  bisulphide,  TiS2. 

Decomp.  slowly  on  moist  air.  Insol.  in 
HC1  or  dil.  H2SO4+Aq.  (Ebelmen.) 

Sol.  in  aqua  regia  or  HNO3+Aq.  Decomp. 
by  KOH+Aq  or  NaOH+Aq.  Insol.  in 
KSH+Aq.  (Rose.) 

Sol.  in  HF  at  100°.  (v.  der  Pfordten,  A. 
234.  257.) 

Titanium  sesgwisulphide,  Ti2S3. 

Insol.  in  caustic  alkalies +Aq.  Sol.  in  HF 
at  a  high  temp.  Insol.  in  aqua  regia.  (v.  der 
Pfordten,  A.  234.  257.> 

Titanomolybdic  acid,  TiO2,  12Mo03+22H2O. 

Very  sol.  in  H2O. 

Sol.  in  ether.  (Pechard,  C.  ft*  1893,  117. 
790.) 


1084 


TITANOMOLYBDATE,  AMMONIUM 


Ammonium  titanomolybdate, 

2(NH4)2O,  TiO2,  12MoO3+10H2O. 
Sol.  in  H2O  and  acids;  completely  insol. 
in  solutions  of  ammonium  salts.     (Pechard.) 

Potassium  titanomolybdate, 

2K2O,  TiO2,  12Mo03+16H2O. 
Efflorescent. 
Sol.  in  H2O.    (Pechard.) 

Titanodfdtungstic  acid,  H8TiWi0O36+ 

zH20. 
(Lecarme,  Bull.  Soc.  (2)  36.  17.) 

Titanotungstic    acid    or    TitaTioduodeci- 

tungstic  acid,  H8TiW12O42+zH2O 
(Lecarme,  Bull.  Soc.  (2)  36.  17.) 

Titanous  acid. 

Sodium  titanite,  Na3TiO3  =  3Na2O,  Ti203. 

Sol.  in  dil.  acids.  (Koenig  and  v.  der 
Pfordten,  B.  22.  2075.) 

Titanyl  compounds. 
See  Titanium  oxy- compounds. 

Triamine  cobaltic  compounds. 
See  Dichrocobaltic  compounds. 

Trithionic  acid,  H2S3O6. 

Known  only  in  aqueous  solution. 

Solution  in  H2O  gradually  decomposes  in 
the  cold,  rapidly  at  80°.  Not  decomp.  if  very 
dilute  or  in  presence  of  acids,  except  HNO3, 
HC1O3,  and  HIO3.  (Fordos  and  Gelis,  A.  ch. 
(3)  28.  451.) 

Trithionates. 

The  trithionates  are  all  sol.  in  H2O,  and 
very  easily  decomposed. 

Ammonium  trithionate,  (NH4)2S3O6. 

Very  deliquescent  and  unstable. 

Very  sol.  in  H2O. 

Insol.  in  abs.  alcohol.  (Divers  and  Ogawa, 
Chem.  Soc.  1900,  77.  337.) 

Barium  trithionate,  BaS3O6+2H2O. 

Very  sol.  in  H2O.  Precipitated  from 
aqueous  solution  by  large  excess  of  alcohol. 
Aqueous  solution  is  very  unstable.  (Kessler 
Pogg.  74.  250.) 

Lead  trithionate,  PbS3O6. 

Very  si.  sol.  in  H2O.  Sol.  in  Na2S2O3+Aq 
(Fogh,  C.  R.  HO.  524.) 

Potassium  trithionate,  K2S3O6. 

Sol.  in  H2O.  Insol.  in  alcohol.  (Kessler, 
Pogg.  74.  270.) 

Sol.  in  H2O  with  decomp. 

Insol.  in  alcohol.  (Langlois,  A.  1841,  40. 
102.) 


Sodium  trithionate,  Na2S3O6. 
Very  sol.  in  H2O. 
+3H2O.    (Villiers,  C.  R.  106.  1356.) 

Thallous  trithionate,  T12S3O6. 

Sol.  in  H2O.    (Bevan,  C.  N .  38.  294.) 
Zinc  trithionate. 

Sol.  in  H2O,  but  decomposes  upon  warming 
the  solution.  (Fordos  and  Gelis,  C.  R.  16. 
1070.) 

Tungsten,  W. 

Metallic.  Not  attacked  by  heating  with 
fuming  HNO3,  aqua  regia.  or  other  acids,  or 
by  boiling  KOH  +  Aq.  Sol.  in  KOH  +  Aq  and 
NaClO+Aq.  (v.  Uslar,  A.  94.  255.) 

Not  easily  acted  upon  by  moist  air,  if  no 
CO2  present.  Sol.  in  a  mixture  of  HF  and 
HNO3.  Very  slowly  sol.  in  H2SO4,  HC1  and 
HF.  (Moissan,  C.  R.  1896,  123.  15.) 

Very  slowly  attacked  by  HNO3,  H2SO4, 
HC1  and  even  CrO3.  A  mixture  of  CrO3  and 
H2SO4  dissolved  1.67  g.  in  16  hrs.  from  a  fine 
wire  and  1.36  g.  in  14  hours.  (Fink,  Met. 
Chem.  Eng.  1910,  8.  341.) 

Compact  tungsten  is  not  attacked  by  dil., 
and  only  si.  dissolved  by  cone.  H2SO4.  Not 
attacked  by  dil.  or  cone.  HC1.  HNO3  and 
HNO3+HC1  attack  slowly  by  long  heating, 
forming  thin  layer  of  WO3.  Slowlv  sol.  in 
HNO3+HF.  (Weiss,  Z.  anorg.  1910,  65.  339.) 

Aluminothermic  tungsten  is  insol.  in 
acids  and  in  aqua  regia.  Sol.  in  fused  KOH. 
(Stavenhagen,  B.  1899,  32.  1515.) 

Insol.  in  HC1  of  any  concentration  at  room 
temp,  and  only  very  si.  sol.  at  110°.  After 
being  in  contact  with  hot  cone.  HC1  (sp.  gr. 
1.15)  for  175  hrs.  the  metal  lost  0.5%  of  its 
weight.  SI.  sol.  in  dil.  HC1  at  110°. 

Insol.  in  cone.  H2SO4  at  room  temp,  and 
in  dil.  H2SO4  at  110J.  Somewhat  sol.  in  cone. 
H2S04  at  high  temp. 

Insol.  in  cone.  HNO3,  and  hot  or  cold  HF. 

SI.  sol.  in  aqua  regia. 

Very  sol.  in  HF+HNO3.  (Ruder,  J.  Am. 
Chem.  Soc.  1912,  34.  387.) 

Insol.  in  aqua  regia  and  acids;  sol.  in  fused 
KOH.  (Stavenhagen,  B.  1899,  32.  1514.) 

Insol.  in  KOH-f-Aq. 

Sol.  in  fused  KOH. 

Slowly  sol.  in  fused  Na2CO3,  K2CO3  or 
mixture  of  the  two. 

Somewhat  sol.  in  NaOCl+Aq.  (Ruder,  J. 
Am.  Chem.  Soc.  1912,  34.  388.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  .20.  830.) 

Crystalline.  Insol.  in  H2O,  HC1,  or  H2SO4. 
Oxidised  by  HNO3  or  aqua  regia.  (D'Elhu- 
jar.) 

Sol.  in  boiling  KOH+Aq.  (Riche,  A.  ch. 
(3)  50.  5.) 

Amorphous.  Easily  oxidised  by  HNO3  + 
Aq.  (Zettnow.) 

Tungsten  amide. 
See  Tungsten  nitride. 


TUNGSTEN  IODIDE 


1085 


Tungsten  arsenide,  WAs2. 

Insol.  in  H2O  and  other  solvents.  Not 
attacked  by  boiling  HF  or  HNO3.  Sol.  in 
cold  HF+HNO3  and  in  hot  aqua  regia.  Not 
attacked  by  hot  KOH+Aq  or  NaOH+Aq. 
Decomp.  by  fused  KOH  or  NaOH.  (De- 
facqz,  C.  R.  1901,  132.  139.) 

Tungsten  boride,  WB2. 

Slowly  attacked  by  cone,  acids;  vigorously 
attacked  by  aqua  regia.  (Tucker  and  Moody. 
Chem.  Soc.  1902,  81.  16.) 

Tungsten  ^'bromide,  WBr2. 

Partly  sol.  in  H2O,  the  rest  decomposing  to 
W02  and  HBr. 

Tungsten  pentdbromide,  WBr5. 

Decomp.  by  moist  air  or  H2O.  Sol.  in 
caustic  alkalies  +Aq. 

Very  hydroscopic.    Fumes  in  the  air. 

Decomp.  by  H2O. 

Sol.  in  HF,  or  cone.  HC1.  SI.  sol.  in  fuming 
HBr.  Decomp.  by  dil.  HC1,  cone.  HNO3  or 
dil.  H2SO4.  Readily  attacked  by  fused 
alkalies  or  alkalies +Aq.  Sol.  in  CC14,  CHC13, 
CHBr3,  abs.  alcohol,  ether,  essence  of  tere- 
benthine  and  benzene.  (Defacqz,  C  R 
1899,  128.  1232.) 

Tungsten  /lezabromide,  WBr6. 

Decomp.  by  H2O  and  in  the  air. 

Sol.  in  NH4OH+Aq.  (Smith,  J.  Am. 
Chem.  Soc.  1897,  18.  1100.) 

Tungsten  bromochloride,  WC16,  WBr6. 

Decomp.  by  H2O.  Sol.  in  HF.  Decomp. 
by  HNO3  or  H2SO4.  Violently  attacked  by 
fused  alkali  or  alkali +Aq.  Sol.  in  most 
organic  solvents. 

WC16,  3WBr6.  Properties  like  those  of 
WC16,  WBr6.  (Defacqz,  C.  R.  1899,  129.  516.) 

Decomp.  by  H2O.  Sol.  in  40%  HF+Aq. 
22°  B.  HC1  +Aq  gives  a  si.  ppt.  of  WO3. 
Decomp.  by  HNO3  and  by  H2SO4.  Sol.  in 
abs.  alcohol,  ether,  CS2,  C6H6  and  glycerine. 
Sol.  in  CC14  only  on  warming.  Nearly  insol. 
in  oil  of  turpentine.  (Defacqz.) 

Tungsten  bronze. 

See— 


Tungstate 
Tungstate 

slum. 
Tungstate 
Tungstate 

slum. 
Tungstate 
Tungstate 
Tungstate 

slum. 
Tungstate 
Tungstate 


tungsten  oxide,  barium, 
tungsten  oxide,  barium  potas- 

tungsten  oxide,  barium  sodium, 
tungsten  oxide,  calcium  potas- 

tungsten  oxide,  calcium  sodium, 
tungsten  oxide,  lithium, 
tungsten  oxide,  lithium  potas- 

tungsten  oxide,  potassium, 
tungsten  oxide,  potassium  so- 


Tungstate  tungsten  oxide,  potassium  stron- 
tium. 

Tungstate  tungsten  oxide,  sodium. 

Tungstate  tungsten  oxide,  sodium  stron- 
tium, 

Tungsten  carbide,  W2C. 

Sol.  in  boiling  HNO3;  very  slowly  acted 
upon  by  other  acids.  (Moissan,  C.  R.  1896, 
123.  16.) 

WC.  Insol.  in  dil.  acids;  only  si.  sol.  in 
H2SO4  and  cone.  HNO3;  sol.  in  fused  KC1O3 
and  KNO3.  (Williams,  C.  R.  198,  126.  1724.) 

Tungsten  bichloride,  WC12. 

Decomp.  on  the  air  or  with  H2O.    (Roscoe.) 

Tungsten  fefrachloride,  WC14. 

Deliquescent.  Partly  sol.  in  H2O,  with  sub- 
sequent decomposition.  (Roscoe.) 

Tungsten  pentachloride,  WC16. 

Very  deliquescent.  Decomp.  with  H2O 
with  hissing  and  evolution  of  heat  and  separa- 
tion of  W2O5. 

Very  si.  sol.  in  CS2.    (Roscoe.) 

Tungsten  Aermchloride,  WC16. 

Not  decomp.  by  moist  air  or  H2O.  De- 
comp. by  alcohol.  Very  sol.  in  CS2.  (Ros- 
coe.) 

Easily  sol.  in  PGC13.    (Teclu,  A.  187.  255.) 

Tungsten  chloride  nitrogen  sulphide,  WC14, 


(Davis,   Chem.   Soc.  1906,  89.    (2)    1575.) 

Tungsten  chloroarsenide,  W2AsCl9. 

Hydroscopic;  decomp.  by  H2Q  and  acids; 
sol.  in  aq.  solution  of  alkalies;  insol.  in  an- 
hydrous organic  solvents.  (Defacqz,  C.  R. 
1901,  132.  139.) 

Tungsten  chlorosulphide,  W2S7C18. 

Decomp.  by  H2O. 

Sol.  in  S2C12.  (Smith  and  Oberholtzer,  Z. 
anorg.  1894,  5.  68.) 

WC1C,  3WS3.  Decomp.  by  H2O.  Insol.  in 
CS2,  alcohol  and  C6H6.  (Defacqz,  A.  ch.  1901, 
(7)  22.  266.) 

Tungsten  /z&rafluoride,  WFfl. 

Fumes  in  the  air. 

Decomp.  by  H2O.  Easily  sol.  in  aq.  alkalies. 
(Ruff,  B.  1905,  38.  747.) 

Tungsten  duodide,  WI2. 

Not  decomp.  by  H2O.  (Roscoe,  A.  162. 
366.) 

Insol.  in  H2O,  CS2  and  alcohol.  Decomp. 
by  boiling  H2O,  HNO3,  H2SO4  and  aqua 
regia;  sol.  in  fused  KOH,  and  alkali  carbon- 
ates. (Defacqz,  C.  R.  1898,  126.  936.) 


1086 


TUNGSTEN  IODIDE 


Tungsten  Zdraiodide,  WI4. 

Insol.  in  H2O,  ether,  chloroform  and  tur- 
pentine; sol.  in  abs.  alcohol;  decomp.  when 
boiled  with  H2O;  sol.  with  decomp.  in  dil. 
HC1  and  H2SO4,  in  HNO3  and  aqua  regia,  and 
in  alkali  hydroxides  and  carbonates  fused  or 
in  aq.  solution.  (Defacqz,  C.  R.  1898,  127. 
511.) 

Tritungsten  nitride,  W3N2. 

(Uhrlaub.) 

W2N3.  Insol.  in  HNO3,  dil.  H2SO4  and 
NaOH+Aq.  (Rideal,  Chem.  Soc.  1889,  55. 
44.) 


Tungsten   nitride   amide,   W3N6H4 

W(NH2)2. 

Not  attacked  by  acids  or  caustic  alkalies  + 
Aq.  (Wohler,  A.  '73.  191.) 

Tungsten  nitride  amide  oxide,  W7N8H4O4  = 
3WN2,  W2(NH2)2,  2WO3. 

Not  attacked  by  acids  or  alkalies.  (Woh- 
ler.) 

Tungsten  worzoxide,  WO. 

Insol.  in  H2O.  Not  attacked  by  HC1, 
HF,  H2SO4,  or  KOH+Aq.  HNO3+Aq  or 
aqua  regia  convert  it  into  WO3.  (Headden, 
Sill.  Am.  J.  146.  280.) 

Tungsten  dioxide,  WO2. 

(a)  When  prepared  in  the  dry  way,  is  at- 
tacked only  by  aqua  regia,  which  oxidises  to 
WO3. 

(6)  When  moist,  is  sol.  in  HC1  or  H2SO4  + 
Aq,  also  in  KOH+Aq.  Insol.  in  NH4OH+ 
Aq.  (Riche,  A.  ch.  (3)  60.  5.) 

Cryst.  Insol.  in  HC1,  H2SO4  and  cone.  aq. 
alkalies;  sol.  in  HNO3.  (Hallopeau,  C.  R. 
1898,  127.  135.) 

Tungsten  oxide,  blue. 

W2O6  (Riche,  A.  ch.  (3)  60.  33);  W3O8  (v. 
Uslar);  W4On  (Gmelin). 

All  are  probably  the  same  substance.  Not 
attacked  by  boiling  HNO3  or  aqua  regia. 
Slowly  sol.  in  boiling  KOH+Aq. 

Tungsten  inoxide,  WO3. 

Insol.  in  H2O  or  acids.  SI.  sol.  in  dil.  KOH 
+Aq,  NaOH+Aq,  Na2CO3+Aq,  or  H2CO3  + 
Aq,  but  easily  sol.  in  cone,  boiling  solutions 
of  same.  NH4OH+Aq  when  boiling  has  a 
solvent  action. 

Insol.  in  cone,  and  dil.  H2SO4.  (Desi  J 
Am.  Chem.  Soc.  1897,  19.  214.) 

Min.  Tungstite.  Insol.  in  acids.  Sol.  in 
NH4OH+Aq. 

Tungsten  oxide,  W2O8. 

Sol.  in  alkalies.  (Desi,  J.  Am.  Chem.  Soc. 
1897,  19.  214.) 


W3O8.  Insol.  in  acids  and  alkalies.  (Desi, 
J  Am.  Chem.  Soc.  1897,  19.  228.) 

+H2O.  Like  W5O14+H2O.  (Allen  and 
Gottschalk,  Am.  Ch.  J.  1902,  27.  336.) 

W4O3.  (Desi,  J.  Am.  Chem.  Soc.  1897,  19. 
219.) 

W5O9.     (Desi.) 

W5Oi4+H2O.  Insol.  in  H2O  containing  a 
little  HC1. 

Slowly  attacked  by  cold,  cone.  MOH+Aq. 
(Allen 'and  Gottschalk,  Am.  Ch.  J.  1902,  27. 
333.) 

Tungsten  tfn'oxide  ammonia,  WO3,  3NH3. 

(Rosenheim  and  Jacobsohn,  Z.  anorg. 
1906,  50.  306.) 

Tungsten  oxybromide,  etc. 
See  Tungstyl  bromide,  etc. 

Tungsten  rao/iophosphide,  WP. 

Not  attacked  by  HF  or  HC1. 

Sol.  in  warm  HNO3+HF.  Slowly  attached 
by  hot  HNO3. 

Not  attacked  by  KOH+Aq  or  NaOH+Aq. 
(Defacqz,  C.  R.  1901,  132.  34.) 

Tungsten  efo'phosphide,  WP2. 

Insol.  in  H2O  and  in  most  organic  solvents; 
insol.  in  HC1  and  HF;  sol.  in  a  mixture  of 
HF  and  HNO3  in  the  cold,  and  in  aqua  regia 
on  warming.  (Defacqz,  C.  R.  1900,  130.  916.) 

Tungsten  phosphide,  W4P2. 

Not  attacked  by  any  acid,  not  even  by 
aqua  regia.    (Wohler  and  Wright,  A.  79.  244.) 
W3P4.    (Wohler  and  Wright.) 

Tungsten  cfo'selenide,  WSe2. 
(Uelsmann.) 

Tungsten  iriselenide,  WSe3. 

Easily  sol.  in  alkali  sulphides  or  selenides 
+Aq.  (Uelsmann,  Jahrb.  f.  Ch.  1860.  92.) 

Tungsten  silicide. 

Sol.  in  HF. 

Only  very  si.  sol.  in  other  acids.  (Warren, 
C.  N.  1898,  78.  319.) 

WSi2.  Not  attacked  by  ordinary  acids  and 
scarcely  by  warm  aqua  regia,  but  violently 
attacked  by  HNO3+HF.  SI.  attacked  by 
10%  alkalies +Aq.  (Honigschmid,  M.  1907, 
28.  1017.) 

Not  attacked  by  dil.  or  cone.  HC1,  HF, 
HNO3  or  H2SO4,  nor  by  not  aqua  regia.  . 

Attacked  by  HNO3+HF  or  by  fused 
alkalies.  (Defacqz,  C.  R.  1907,  144.  850.) 

WSi3.  Violently  attacked  by  HNO3+HF. 
Not  attacked  by  HNO3,  H2SO4,  HC1  or  HF. 
(Frilley,  Rev.  Me*t.  1911,  8.  509.) 

W2Si3.  Insol.  in  acids  including  HF;  sol. 
in  a  mixture  of  HF  and  HNO3;  sol.  in  fused 
alkali  hydroxides  and  carbonates.  (Vigour- 
oux,  C.  R.  1898,  127.  394.) 


TUNGSTATE,.  ALUMINUM  AMMONIUM 


1087 


Tungsten  ^sulphide,  WS2. 

Oxidised  by  HNO3+Aq.     (Berzelius.) 

Insol.  in  min.  acids. 

Sol.  in  a  mixture  of  HF  and  HNO3  and  in 
fused  alkalies  and  alkali  carbonates.  (De- 
facqz,  C.  R.  1899,  128.  611.) 

Tungsten  Znsulphide,  WS3. 

Somewhat  sol-,  in  cold,  abundantly  in  hot 
H2O,  but  separated  out  by  the  addition  of 
salts,  especially  NH4C1,  or  acids.  Sol.  in 
alkali  sulphides,  and  hydrosulphides+Aq. 
Sol  in  caustic  alkalies,  and  alkali  carbonates 
+Aq.  Slowly  sol.  in  NH4OH+Aq  in  the 
cold. 

Tungstic  acid,  H2WO4. 

Insol.  in  H2O.  Sol.  in  HF.  Insol.  in  tung- 
states+Aq. 

44.7%  H2WO4  is  sol.  in  50%  HF+Aq  at 
25°. 

55.3%  H2WO4  is  sol.  in  50%  HF  +Aq  at 
50°. 

100  g.  sat.  H2WO4+HCl+Aq  contain 
0.68  g.  H2WO4  at  80°. 

9.8  %  H2WO4  is  sol.  in  sat.  alcoholic  HC1 
at  75°. 

Insol.  in  alcoholic  solutions  of  HBr  and  HI. 
(Rosenheim,  Chem.  Soc.  1911,.  100.  (2)  402.) 

Freshly  pptd.  tungstic  acid  dissolves  in 
H2O2.  (KeUner,  Dissert.  1909.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  830.) 

H4WO5.  Precipitate.  SI.  sol.  in  H2O  and 
aqueous  solutions  of  the  tungstates.  Sol.  in 
250-300  p'ts.  H2O.  When  freshly  pptd.,  sol. 
in  alkali  hydrates  or  carbonates +Aq.  (An- 
thon,  J.  pr.  9.  6.) 

Metatungstic  acid,  H2W4O18+9H2O. 

Sol.  in  H2O.  Solution  may  be  boiled  and 
evaporated  to  a  syrupy  consistency,  when  it 
suddenly  gelatinises  and  ordinary  tungstic 
acid  is  precipitated. 

Sol.  in  H20.  When  heated  to  50°,  it  be- 
comes insol.  in  H2O.  (SobolefT,  Z.  anorg. 
1896,  12.  28.) 

Solubility  in  H2O  at  t°. 


t° 

100  ccm.  ether  dissolve 
g.  of  the  cryst.  acid 

0 

7.8 
18.2 
24.3 

83.456 
88.389 
99.66 
110.76 

t° 

100  ccm.  H2O  dis- 
solve g.  of  the  cryst. 
acid 

Sp.  gr.  of  the 
solution 

0 
22 
43.5 

41.46 
88.57 
111.87 

1.6025 
2.5239 
3.6503 

(Soboleff.) 

Sp.  gr.  of  solution  of  metatungstic  acid  at 
17.5°  containing: 

2.79       12.68      27.61      43.75%  WO8. 
1.0257     1.1275     1.3274     1.6343 
(Scheibler,  J.  pr.  83.  273.) 


Sp.  gr.  of  aqueous  solution  calculated  by 
M  =  Mendelejeff,  and  G  =  (Gerlach  (Z.  anal. 
27.  300),  containing: 

5         10         15         20        25%  W03, 
M    1.047     1.098     1.153     1.214     1.285 
G    1.0469  1.0980  1.1544  1.2172  1.2873 

30         35         40         45        50%  W0». 
M    1.366    1.458      1.555     1.581  (?) 
G    1.3660  1.4540  1.5527  1.6630  1.7860 

Solubility  in  ether  at  t°. 


(Soboleff,  Z.  anorg.  1896,  12.  32.) 

Colloidal.  Sol.  in  H2O.  Not  precipitated 
by  acids  or  alcohol.  Can  be  evaporated  to 
dryriess  and  heated  to  200°,  and  still  remains 
sol.  in  H2O.  Sol.  in  J^pt.  of  H2O. 

Sp.  gr.  of  aqueous  solution  containing: 
5          20          50         66.5      79.8%  WO,. 
1.0475    1.2168    1.8001   2.596     3.243 
(Graham,  Chem.  Soc.  17.  318.) 

Perhaps  paratungstic  acid,  Hi0Wi2O4i. 
(Klein,  Bull  Soc.  (2)  36.  547.) 

Tungstates. 

Few  normal  tungstates  are  sol.  in  H2O, 
even  some  of  the  K  and  NH4  salts  are  very 
si.  sol.  Most  of  the  metatungstates,  however, 
are  easily  sol.  in  H2O. 

Tungstates  insol.  in  H2O  are  usually  insol. 
in  dil.  acids. 

Aluminum  tungstate,  Al2(WO4)8-f  8H2O. 

Precipitate.  Insol.  in  H2O  and  Na2WO4+ 
Aq.  Sol.  in  (NH4)2Al2(SO4)4+Aq,  NaOH  + 
Aq,  NH4OH+ Aq. 

Easily  sol.  in  H3PO4,  H2C2O4,  and 
H2C4H4O6+Aq.  (Lotz,  A.  83.  65.) 

Sol.  in  1500  pts.  H2O  at  15°.  (Lefort,  C.  R. 
87.  748.) 

Al2Oa,  4WO3+9H2O.  Sol.  in  400  pts.  H2O 
at  15°.  (Lefort,  C.  R.  87.  748.) 

A12O3,  5WO3+6H2O.  Sol.  in  H2O,  from 
which  it  is  pptd.  by  alcohol.  (Lefort.) 

Formula  according  to  Lefort  is  A12O3)  3WO8 
+3H20,  2W03. 

See  also  Aluminicotungstic  acid. 

Aluminum  paratungstate,   5A12O3,  36WO«-f 

46H20=A1203,  7W08+9H20  (?). 
Easily  sol.  in  an  alum  solution.     (Lotz,  A. 
83.  65.) 
Aluminum  ammonium  tungstate,  3(NH4)2O, 

A12O8,  9WO8+4H2O. 

Sol.  in  cone.  HNO3  and  in  cone.  HC1. 
(Balke  and  Smith,  J.  Am.  Chem.  Soc.  1903, 
25.  1230.) 


1088 


TUNGSTATE,  ALUMINUM  AMM.ONIUM  ANTIMONY 


Aluminum  ammonium  antimony  tungstate. 

See  Aluminicoantimoniotungstate,  ammon- 
ium. 

Aluminum  antimony  tungstate. 

See  Aluminicoantimoniotungstic  acid. 

Aluminum  zinc  tungstate.  A12O3,  ZnO,  9WO8 
+20H20. 

Very  sol.  in  H2O.  (Daniels,  J.  Am.  Chem. 
Soc.  1908,  30.  1850.) 

2A12O8,  3ZnO,  18WO3  +  16H2O.  Sol.  in 
much  H2O. 

Sol.  in  very  dil.  mineral  acids  or  in  acetic 
acid.  (Daniels.) 

Ammonium  tungstate,  (NH4)2WO4. 
Known  only  in  solution. 

(NH4)4W39n+3H2O  =  2(NH4)2O,  3WO3-f- 
3H2O.  Sol.  in  H2O  with  decomp.  Decomp. 
on  air  with  evolution  of  NH3,  and  formation 
of  paratungstate.  Sol.  in  NH4OH+Aq. 
(Marignac,  A.  ch.  (3)  69.  23.) 

(NH4)4W6017+5H20  =  2(NH4)20,  5WO.+ 
5H2O.  Sol.  at  ordinary  temp,  in  26-29  pts. 
H2O  with  partial  decomposition.  (Marignac.) 

+2y2K20,  +3H20,  +4H20,  +4^H2O, 
and  +5H2O.  (Pinagel,  Dissert,  1904.) 

(NH4)6W3027+8H20  =  3(NH4)20,  8WO3-f 
8H2O.  Sol.  in  H2O.  (Marignac.) 

Colloidal.  (NH4)2O,  6WO3+4  or  6H2O. 
Miscible  with  water  in  nearly  all  propor- 
tions. (Taylor,  J.  Am.  Chem.  Soc.  1902,  24. 
632.) 

Ammonium  raetatungstate,  (NH4)2W4Oi8. 
+6H2O.  (Marignac,  A.  ch.  (4)  3.  74.) 
+8H2O.  Efflorescent.  Very  sol.  in  H2O. 
1  pt.  dissolves  at  15°  in  0.84  pt.  H2O.  (Lotz.) 
1  pt.  dissolves  at  ordinary  temp,  in  0.35 
pt.  H2O.  (Riche.) 

Solubility  increases  rapidly  with  the  tem- 
perature. 

Saturated  solution  at  40°  is  solid  on  cooling. 
SI.  sol.  in  ordinary,  insol.  in  absolute  alcq- 
hol.     (Lotz.)     Insol.  in  ether.     (Riche.) 
[(NH4)2W3Ou>+5H2O  of  Margueritte.j 
(NH4)6Wi6O6i  +  17H2O  =  3(NH4)2O,  16WO3 
+  17H2O.  Very  efflorescent.  Decomp.  by  dis- 
solving in  pure  H2O.     (Marignac,  A.  ch.  (4) 
3.  75.) 

Ammonium  paratungstate,  (NH4)ioWi2O4i  = 
5(NH4)20,  12W08. 

(Marignac,  A.  ch.  (3)  69.  25.) 

According  to  Lotz  (A,  91.  49)  and  Scheibler 
(J.  pr.  80.  208),  formula  is  (NH4)6W7O24  = 
3(NH4)20,  7W03. 

+5H2O.    (Scheibler.  J.  pr.  48.  232.) 

+  11H2O.  Sol.  in  25-28  pts.  cold  H2O 
(Anthon.) 

Sol.  in  26.1  pts.  H2O  at  10.7°,  and  5.8  pts 
at  100°.  (Lotz.) 

Sol.  in  33.3  pts.  cold  H2O,  and  9.6  pts  at 
100°.  (Riche.) 


Sol.  in  22-38  pts.  H2O  at  15-18°.  The 
solution  gradually  decomposes,  with  the 
"ormation  oi  a  more  soluble  salt.  (Marignac.) 

Not  much  more  sol.  in  NH4OH+Aq  than 
n  H2O.  Insol.  in  alcohol.  (Anthon.) 

Sol.   in   H2O2.      (Kellner.    Dissert,    1909.) 

Ammonium  bismuth  tungstate. 
See  Bismuthicotungstate,  ammonium. 

Ammonium  cadmium  para  tungstate, 

3(NH4)20,  12CdO,  35WO3+35H2O. 
Ppt.    Sol.  in  H2O  acidulated  with  HNO3. 
(Lotz,  A.  91.  49.) 

Ammonium  cerium  tungstate. 
See  Cericotungstate,  ammonium. 

Ammonium  cobaltous  tungstate,  8(NH4)2O, 

2CoO,  15WO3+3H2O. 
(Carnot,  C.  R.  109.  147.) 

Ammonium  hydroxylamine  tungstate, 

NH4OWO4NH4. 

Sol.  in  H2O.  (Hofmann,  Z.  anorg.  1898, 
16.  465.) 

Ammonium  iron  (ferric)  tungstate,  5(NH4)2O, 

Fe2O3,  5WO3+5H2O. 
Sol.  in  H2O.     (Borck.) 

Ammonium  lanthanum  tungstate. 
See  Lanthanicotungstate,  ammonium. 

Ammonium  magnesium  p7ratungstate, 
2(NH4)2O,  3MgO,  12WO3+24H2O. 

Very  slightly  sol.  in  H2O.  (Marignac,  A. 
ch.  (3)  69.  58.) 

(NH4)20,  2MgO,  7WO3+10H2O.  Very 
si.  sol.  in  H2O  ;  sol.  in  H2O  acidulated  with 
HNO3.  (Lotz.) 

Ammonium  mercuric  tungstate,  (NH4)2W04, 

HgW04+H20. 

Insol.  in  H2O.  Decomp.  by  acids  or  al- 
kalies. (Anthon.) 

Ammonium  neodymium  tungstate. 
See  Neodymicotungstate,  ammonium. 

Ammonium  nickel  tungstate. 
See  Nickelicotungstate,  ammonium. 

Ammonium  potassium  paratungstate. 

5K(NH4)0,  12W03+HH20. 
Sol.  in  boiling  H2O;  si.  sol.  in  cold  H2O. 
(Hallopeau,  C.  R.  1896,  123.  180.) 

Ammonium  potassium  sodium  paratungstate, 

5(K,  Na,  NH4)20, 12WO3+13H2O,  where 
K:Na:NH4=3:3:4. 
10(K,  Na,  NH4)2O,  24WO3+26H2O,  where 
K  :Na:NH4  =  3:3  : 14.     (Laurent.) 


TUNGSTATE,  CADMIUM 


1089 


Ammonium  sodium  psr?atungstate,  4(NH4)2O, 
Na2O,  12WO3+5H2O. 

Can  be  crystallised  from  H2O  without 
decomp.  (Lotz,  A.  91.  57.) 

+  14H2O.  Sol.  in  warm  H2O.  (Hallopeau, 
C.  R.  1896,  123.  181.) 

(NH4)2O,  4Na2O,  12WO3-f  25H2O.  SI.  sol. 
in  H2O.  (Hallopeau,  C.  R.  1895,  120.  1344.) 

5Na2O,  15(NH4)2O.  48WO3+48H2O. 
(Marignac,  A.  ch.  (3)  69.  53.) 

2Na2O,  3(NH4)2O,  12WO3  +  15H20. 
(Marignac.) 

3(NH4)2O,  2Na2O,  12WO3+15H2O. 

3(NH4)2O,  3Na2O,  16WO3+22H2O.  Sol. 
in  H2O  without  decomp.  (Hallopeau,  C.  R. 
1896,  123.  181.) 

3Na2O,  4(NH4)2O,  16WO3+18H2O. 
(Gibbs,  Am.  Ch.  J.  7.  236.) 

Is  2Na2O,  3(NH4)2O,  12WO3  +  13H2O,  ac- 
cording to  Knorre  (B.  19.  823). 

Very  sol.  in  hot  H2O.  (Knorre,  B.  1886, 
19.  823.) 

(NH4)2O,  3Na2O,  16WO3+38H2O.  (Wy- 
rouboff,  Bull.  Soc.  Min.  1892,  16.  85.) 

6(NH4)2O,  2Na2O,  20WO3+24H2O.  Can 
be  cryst  from  boiling  H2O.  (Baragiola,  Dis- 
sert, '1902.) 

4Na2O,  16(NH4)2O,  50WO3+50H20.  SI. 
sol.  in  cold  H2O.  (Gibbs,  Proc.  Am.  Acad. 
15.  12.) 

Ammonium    zinc    paratungstate,    (NH4)2O, 

2ZnO,  7WO3+13H2O. 
SI.  sol.  in  boiling  H2O,  but  more  easily  on 
addition   of   oxalic,    tartaric,   phosphoric,   or 
dil.  nitric  acids,  or  of  ammonium  tungstate. 
(Lotz,  A.  91.  49.) 

Ammonium  zirconium  tungstate. 
See  Zirconotungstate,  ammonium. 

Ammonium  wetatungstate  nitrate. 
See  Nitrate  raetatungstate,  ammonium. 

Ammonium  tungstate  vanadate. 
See  Vanadiotungstate,  ammonium. 

Antimony  tungstate,  Sb2O3,  5WO3+4H2O. 
Sol.  in  H2O  without  decomp.     (Lefort.) 
Sb2O3,  6WO3+8H2O.     Ppt. 
See  also  Antimoniotungstic  acid. 

Barium  tungstate,  BaWO4. 

Anhydrous.  Insol.  in  H2O.  Decomp.  by 
boiling  HNO3+Aq.  (Geuther  and  Forsberg, 
A.  120.  270.) 

+  3^H2O.  Insol.  in  H2O  or  boiling  H3PO4  + 
Aq.  Sol.  in  boiling,  less  sol.  in  cold  H2C2O4+ 
Aq.  (Anthon.) 

+2^H2O.    Insol.  precipitate.    (Scheibler.) 

Pptd.  BaWO4  is  attacked  by  dil.  acids 
More  sol.  in  NH4NO3+Aq  than  in  H2O 
(Smith  and  Bradbury,  B.  24.  2930.) 


Barium  ^tungstate,  BaW2O7+H2O  (?). 

Nearly  insol.  in  H2O.  100  ccm.  H2O  dis- 
solve about  0.05  g.  at  15°.  (Lefort,  A.  ch. 
(5)  16.  325.) 

Barium  /ntungstate,  BaW3Oi0-|-4H2O  (?). 

Sol.  in  about  300  pts.  H2O  at  15°.  Decomp. 
by  boiling  H2O  into  an  insol.  salt.  (Lefort, 
^  R.  88.  798.) 

+6H2O.     (Scheibler.) 

Barium  me/atungstate,  BaW4O18+9H2O. 

Efflorescent.  Quite  sol.  in  hot  H2O. 
Partly  decomp.  by  cold  H2O  into  BaW3Oio  and 
WO3,  which  recombine  on  heating.  (Schei- 
bler, J.  pr.  80.  204.) 

Barium  tungstate,  BaW8O26+8H2O. 

Insol.   in   H2O  or  HCl+Aq.      (Zettnow.) 
BaW6Oi6.      Barium   bronze.      ( Hallopeau, 

A.  ch.  1900,  (7)  19.  121.) 

Barium  paratungstate,  Ba6Wi2O4i+14H2O, 
or  Ba3W7O24+8H2O. 

Insol.  in  cold  H2O;  when  freshly  pptd.  is 
si.  sol.  in  HNO3+Aq.  (Lotz,  A.  91.  60.) 
Sol.  in  NH4Cl+Aq.  (Wackenroder.) 

+27H2O=Ba3W7O24+16H2O.  Insol.  in 
cold,  si.  sol.  in  hot  H2O.  (Knorre,  B.  18.  327.) 

Barium  potassium  tungstate  tungsten  oxide, 

BaW4Oi2,  5K2W4O12. 
(Engels,  Z.  anorg.  1903,  37.  136.) 

Barium  silver  metotungstate. 

(Scheibler.) 

Barium  sodium  para  tungstate,  2BaO,  3Na2O, 
12  WO3+24H2O.     (Marignac),  or  BaO, 
2Na2O,  7WO3  +  14H2O  (Scheibler). 
Insol.  in  H2O. 

Barium   sodium   tungstate   tungsten   oxide, 

2BaW4012,  3Na2W6015. 
BaW4O12,  5Na2W3O9.     (Engels,   Z.    anorg. 
1903,  37.  131.) 

Bismuth  tungstate,  Bi2O3,  6WO3+8H2O. 

Very  sol.  in  H2O  with  decomp.  Pptd.  by 
alcohol  from  aqueous  solution.  (Lefort,  C.  R. 
87.  748.) 

Cadmium  tungstate,  CdWO4. 

Anhydrous. 

+H2O.  Sol.  in  about  2000  pts.  H2O. 
(Lefort.) 

+2H20.  Insol.  in  H2O.  Sol.  in  hot  phos- 
phoric or  oxalic  acids,  or  in  NH4OH+Aq. 
(Anthon,  J.  pr.  9.  341.) 

Sol.  in  KCN+Aq.  (Smith  and  Bradbury, 
B.  24.  2390.) 


1090 


TUNGSTATE,  CADMIUM 


Cadmium  cfttungstate,  CdW2O7+3H2O  (?). 
Sol.  in  about  500  pts.  H2O  at  15°.    (Lefor 
A.  ch.  (5)  15.  346.) 

Cadmium  fritungstate,  CdW3010+4H2O  (?). 
(Lefort.) 

Cadmium  metotungstate,  CdO,  4W£>3- 
10H2O. 

Not  efflorescent.    (Scheibler,  J.  pr.  83.  273. 

Somewhat  less  sol.  in  HjO  than  the  Mn  sah 
(Wyrouboff.  Bull.  Soc.  Min.  1892,  16.  84. 

Cadmium  para  tungstate,  Cd3W7O24-H6H2O 

Ppt.     (Gonzalez.) 

Insol.  in  H2O.  Sol.  in  NH4OH+Aq,  an 
hot  H3PO4,  H2C2O4.  or  HC2H3O2+Aq. 

Cadmium  sodium  paratungstate,  2CdO,  Na20 

7W03+18H20. 
Difficultly  sol.  in  cold  H2O.     (Knorre,  B 
19.  824.) 

Calcium  tungstate,  CaWO4. 

Insol.  in  H2O  or  dil.  acids.  Sol.  in  aboui 
500  pts.  H2O.  (Lefort.) 

Decomp.  by  KOH+Aq.     (Anthon.) 

When  freshly  pptd.,  sol.  in  NH4Cl+Aq 
(Wackenroder.) 

Sol.  in  Mg,  and  NH4  salts,  also  Na2WO 
+Aq.  (Sonstadt,  C.  N.  11.  97.) 

Min.  Scheelite.  Decomp.  by  HC1  or  HNO; 
+Aq.  with  separation  of  WO3. 

Calcium  ditungstate,  CaW2O7-f  3H2O  (?). 

Sol.  in  30  pts.  H2O  at  15°.  (Lefort,  A.  ch 
(5)  15.  328.) 

Calcium  Zntungstate,  CaW3Oi0+6H2O  (?). 
Sol.  in  cold  H2O.    (Lefort.) 

Calcium  wetatungstate,  CaW4Oi3+10H2O. 
Easily  sol.  in  H2O.    (Scheibler.) 

Calcium  paratungstate,  Ca3W7O24+18H2O  (or 
Ca6Wi2O41+30H2O). 

Much  more  sol.  than  Sr  or  Ba  salt.  (Knorre 
B.  18.  328.) 

Easily  sol.  in  H2O2.  (Knorre,  B.  1885,  18. 
326.) 

Calcium  potassium  tungstate  tungsten  oxide, 

CaW4O12,  5K2W4O12. 
(Engels,  Z.  anorg.  1903,   37.149.) 

Calcium  sodium  paratungstate,  2CaO,  3Na2O 

12W%+3H20. 
(Gonzalez,  J.  pr.  (2)  36.  44.) 

Calcium  sodium  tungstate  tungsten   oxide, 

CaW4012,  5Na2W6016. 
Engels,  Z.  anorg.  1903,  37.  145.) 


Cerium  tungstate,  Ce2(WO4)3+H2O. 

Precipitate.  (Cossa  and  Zecchino,  Gazz. 
ch.  it.  10.  225.) 

Cerium    raetatungstate,     Ce2O3,     12WO3  + 

30H2O. 
Permanent.      Sol.    in    H2O.      (Scheibler.) 

Cerium  sodium  tungstate,  Ce2Na8(WO4)7. 

Insol.  in  H2O.  Slowly  sol.  in  dil.  acids, 
easily  in  HCl+Aq.  (Hogbom,  Bull.  Soc.  (2) 
42.  2.) 

Ce2(WO4)3,  3Na2WO4.  (Didier,  C.  R.  102. 
823.) 

Cerium     tungstate     chloride,     3Ce2(WO4)8, 

2CeCl3. 
(Didier,  C.  R.  102.  823.) 

Chromic   tungstate,   basic,   Cr2O3.    2WO3+ 

5H20. 

Sol.  in  400  pts.  H2O  at  15°.  (Lefort,  C.  R. 
87.  748.) 

Chromic  tungstate,  Cr2(W04)3+7,  and  13H2O. 

Sol.  in  CrCl3+Aq,  and  in  phosphoric, 
oxalic,  or  tartaric  acids  +Aq.  (Lotz.) 

+3H2O.    (Lefort,  C.  R.  87.  748.) 

Cr2O3,  4WO3+6H2O.  Sol.  in  about  50  pts. 
H2O  at  15°.  (Lefort.) 

Cr2O3,  5WO3.  Not  attacked  by  aqua  regia. 
(Smith  and  Oberholtzer,  Z.  anorg.  5.  63.) 

Chromic  yaratungstate,  Cr2W7O24+9H2O. 

Insol.  in  H2O  or  NH4  paratungsta«te+Aq; 
sol.  in  CrCl3+Aq.  (Lotz.) 

Cobaltous  tungstate,  CoWO4. 

Anhydrous.     Insol.  in  H2O  and  acids. 

+2H2O.  Insol.  in  H2O  and  cold  HNO3  + 
Aq.  SI.  sol.  inH2C2O4+Aq.  Completely  sol. 
n  warm  H3PO4,  HC2H3O2,  or  NH4OH+Aq. 
Anthon,  J.  pr.  9.  344.) 

Sol.  in  about  500  pts.  H2O.     (Lefort.) 

Cobaltous  dztungstate,  CoW2O7  (?). 

+3H2O.      Insol.    in    H2O.      SI.    sol.    in 
I2C2O4+Aq.      Completely    sol.    in    H3PO4, 
HC2H3O2,  or  NH4OH+Aq.     (Anthon.) 

+5H2O.  Sol.  in  about  100  pts.  H2O.  (Le- 
ort.) 

+8H20(?).     (Lefort.) 

Cobaltous  ^tungstate,  CoW3O10+4H2O  (?). 
Sol.  in  H2O.     (Lefort,  C.  R.  88.  798.) 

Cobaltous  wetatungstate,  CoW4Oi3+9H2O. 
Sol.  in  H20.     (Scheibler,  J.  pr.  83.  317.) 

obaltous  paratungstate,  Co3W7O24+25H2O. 
(Gonzalez,  J.  pr.  (2)  36.  44.) 


TUNGSTATE,  LANTHANUM  SODIUM 


1091 


Cobaltous     sojiium     paratungstate,     2CoO 
3Na2O,  12WO3+30H2O. 

(Gonzalez.) 

Cupric  tungstate,  CuWO4. 

+2H20.  Insol.  in  H2O.  Sol.  in  H3PO4 
HC2H3O2,  or  NH4OH+Aq.  Insol.  in  H2C2O 
+Aq.  (Anthon.) 

100  ccm.  H2O  at  15°  dissolve  0.1  g.  (Le 
fort.) 

Cupric  ditungstate,  CuW207  (?). 

+4H2O.  Insol.  in  H2O  and  HNO3.  Sol 
in  NH4OH+Aq.  (Anthon,  J.  pr.  9.  346. 

+5H2O.  Sol.  in  about  300  pts.  H2O.  (Le- 
fort.) 

Cupric  raetatungstate,  CuW4Oi3+llH2O. 
Sol.  in  H2O.     (Scheibler.) 

Cupric  paratungstate,  Cu3W7O24+19H2O. 
Insol.  in  H2O.     (Knorre,  B.  19.  826.) 

Cuprocupric  tungstate,  Cu2W04,  2CuW04. 
Insol.  in  H2O.     (Zettnow,  Pogg.  130.  255.) 

Cupric  sodium  paratungstate, 

Cu3Na6(W7O24)2+32H2O. 
Ppt.     (Knorre,  B.  19.  826.) 
CuO,4Na20,  12WO3+32H2O.    Ppt.    (Gon- 
zalez, J.  pr.  (2)  36.  52.) 

Cupric  tungstate  ammonia.  CuWO4.  2NH3  + 
H20. 

(Schiff,  A.  123.  39.) 

CuWO4,  4NH3.  Gives  off  NH3  at  ord. 
temp.  Sol.  in  H2O.  Sol.  in  dil.  NH4OH  + 
Aq.  (Briggs,  Chem..  Soc.  1904,  85.  676.) 

CuO,  4WO3,  6NH3+8H2O.  Insol.  in  H2O. 
Nearly  insol.  in  dil.  NH4OH+Aq.  (Briggs, 
Chem.  Soc.  1904,  85.  676.) 

Didymium  tungstate,  Di2(WO4)3. 

Precipitate.  (Frerichs  and  Smith,  A.  191. 
355.) 

Didymium  wetotungstate. 
Sol.  in  H2O.     (Scheibler.) 

Didymium  sodium  tungstate,  DiNa3(WO4)3. 

Insol.  in  H2O.  Slowly  sol.  in  dil.  acids. 
Sol.  in  cone.  HCl+Aq. 

DiNa(WO4)2.  As  above.  (Hogbom,  Bull. 
Soc.  (2)  42.  2.) 

Erbium  sodium  tungstate,  Na6Er4(W04)9. 
Insol.  in  H2O.     (Hogbom.) 

Glucinum  metatungstate. 
Very  sol.  in  H2O. 

Indium  tungstate,  In2(WO4)3+8H2O. 

Insol.  in  H2O.  Decomp.  by  acids.  (Renz, 
Dissert.  1902.) 


Iron  (ferrous)  tungstate,  FeW04. 

Min.  Ferberite,  Reinite. 

+3H2O.  Insol.  in  H2O.  Sol.  in  cold 
H2SO4,  HC1,  or  HNO3+Aq.  Decomp.  by 
boiling  acids  with  separation  of  WO3.  Sol.  in 
boiling  H3PO4+Aq  or  warm  H2C2O4+Aq. 
(Anthon,  J.  pr.  9.  343.) 

+zH2O.  Very  unstable.  (Lefort,  A.  ch. 
(5)  15.  314.) 

Iron  (ferrous)  ditungstate,  FeW2O7  (?). 

Insol.  in  H2O.  Sol.  in  hot  H3PO4+Aq  or 
H2C2O4+Aq.  Decomp.  by  dil.  HCl+Aq  or 
by  KOH+Aq.  (Ebelmen,  C.  R.  17.  1198.) 

+zH2O.    Very  unstable.    (Lefort.) 

Iron      (ferrous)     Zn'tungstate,      FeW8Oi0+ 

Ppt.     Decomp.  by  cold,  more  rapidly  by 

hotH2O.    (Lefort.) 

Iron  (ferrous)  raetatungstate. 

Sol.  in  H2O.     (Scheibler,  J.  pr.  83.  315.) 

Iron  (ferric)  tungstate,  basic,  Fe2O3,  2W03+ 


Sol.  in  about  50  pts.  H2O.    (Lefort.) 
2Fe2O3,  3WO3+6H2O.     Sol.  in  about  300 
pts.  H2O  at  15°.    (Lefort.) 

Iron  (ferric)  ^ntungstate  (?),  Fe2O3,  4WO3+ 

4H2O  =  Fe2O3,  3WO3+WO3,  4H2O  (?). 
Sol.   in  H2O  without  decomp.      (Lefort.) 

Iron  (ferric)  wetotungstate. 

Sol.  in  H2O.    (Scheibler,  J.  pr.  83.  273.) 

Iron  (ferrous)  manganous  tungstate,  7FeWC>4, 

MnWO4. 

(Geuther  and  Forsberg,  A.  120.  277.) 
4FeW04,  MnWO4.    (G.  and  F.) 
3FeWO4,  MnWO4.     Partially  sol.  in  cone. 

HCl+Aq.    (G.  andF.) 

3FeWO4,  2MnWO4.    (G.  and  F.) 
FeWO4,   MnWO4.      (Zettnow,   Pogg.   130. 

250.) 

FeWO4,  2MnWO4.    (G.  and  F.) 
FeWO4,  7MnWO4.    (G.  and  F.) 
.rFeWO4,  ?/MnWO4.    Min.  Wolframite.    Sol. 
n  HCl+Aq,  and  boiling  H3PO4+Aq. 

Lanthanum  tungstate,  La2(WO4)3. 
Precipitate. 

Lanthanum  metotungstate. 
Sol.  in  H2O.    (Scheibler.) 

Lanthanum  silver  tungstate. 
See  Lanthanicotungstate,  silver. 

Lanthanum  sodium  tungstate,  Na8La2(WO4)7. 

Insol.  in  H2O.  Slowly  sol.  in  dil.  acids. 
Sol.  in  HCl+Aq. 

La4Na6(WO4)9.  As  above.  (Hogbom, 
Bull.  Soc.  (2)  42.2.) 


1092 


TUNGSTATE,  LEAD 


Lead  tungstate,  PbWO4. 

Insol.  in  H2O  or  cold  HNO3+Aq.  Sol.  in 
KOH+Aq.  Decomp.  by  hot  HNO3+Aq. 
(Anthon,  J.  pr.  9.  342.) 

Sol.   in  about  4000  pts.   H2O.     (Lefort.) 

Min.  Scheelenite,  Stolzite.  Sol.  in  KOH  + 
Aq;  decomp.  by  HNO8. 

Absolutely  insol.  in  NH4NO3+Aq.  (Smith 
and  Bradbury,  B.  24.  2930.) 

Lead  ditungstate,  PbW2O7+2H2O  (?). 
Sol.  in  about  80  pts.  H2O  at  15°.    (Lefort.) 

Lead  Zntungstate,  PbW3O10+2H2O  (?). 
Ppt.    (Lefort.) 

Lead  metotungstate,  PbW4Oi3+5H2O. 

SI.  sol.  in  cold,  more  in  hot  H2O.  Sol.  in 
hot  HNOg+Aq.  (Scheibler,  J.  pr.  83.  318.) 

Lead  paratungstate,  Pb3W7O24. 

Insol.  in  H2O,  dil.  HNO3+Aq,  (NH4)2WO4 
+Aq,  or  Pb(NO3)2+Aq.  Sol.  in  NaOH  + 
Aq  or  boiling  H3PO4+Aq.  (Lotz,  A.  91.  49.) 

Lead   sodium   paratungstate,   PbO,   4Na2O, 

12WO3+28H2O. 
(Gonzalez.) 

Lithium  tungstate,  Li2WO4. 

Rather  easily  sol.  in  H2O.     (Gmelin.) 

Lithium  wetotungstate,  Li2W4Oi3. 

Insol.  in  H2O.     (Knorre,  J.  pr.  (2)  27.  94.) 
+rcH2O.    Syrup.    (Scheibler.) 

Lithium    paratungstate,    Lii0Wi2O41+33H2O 

(orLi6W7O24+19H2O). 
According  to  Scheibler,  more  sol.  than  the 
paratungstates  of  the  other  alkali  metals. 

Lithium  tungstate  tungsten  oxide,  Li2WsOi5. 

Lithium  bronze.    Insol.  in  H20. 

Lithium  potassium  tungstate  tungsten  oxide, 
Li2W5015,  3K2W4012. 

Lithium  potassium  bronze.  Insol.  in  H2O. 
(Feit,  B.  21.  135.) 

Lithium  sodium  tungstate,  Li2WO4+3H2O, 
3(Na2WO4+3H2O). 

(Traube,  N.  Jahrb.  Miner,  1894,  I.  190.) 

Magnesium  tungstate,  MgWO4. 

Anhydrous.  Insol.  in  H2O.  Gradually  de- 
comp. by  boiling  cone.  HNO3+Aq.  (Geuther 
and  Forsberg,  A.  120.  272.) 

+3H2O.  Very  sol.  in  H2O;  nearly  insol 
in  alcohol.  (Lefort,  A.  ch.  (5)  16.  329.) 

+7H2O.  Slowly  sol.  in  cold,  very  easily  in 
hot  H2O.  (Ullik,  W.  A.  B.  56.  2.  152.) 


Magnesium  ^'tungstate,  MgW2O7+8H2O  (?). 
Sol.  in  about  100  pts.  H2O.    (Lefort.) 

Magnesium  Zntungstate,  MgW3Oio+4H2O(?). 
Easily  sol.  in  H2O  with  gradual  decomp. 
Lefort.) 

Magnesium  rae.'atungstate,  MgW4Oi3+8H2O. 
Sol.  in  H2O.    (Scheibler.) 

esium      paratungstate,      Mg3W7O244- 
24H20. 

Very  difficultly  sol.  in  cold,  somewhat  sol. 
n  hot  H2O.  (Knorre,  B.  19.  825.) 

Magnesium   potassium  tungstate,   MgWO4, 

K2WO4. 

+2H2O.    Very  si.  sol.  in  H2O.    (Ullik.) 
+6H2O.    Precipitate. 

Magnesium  potassium  paratungstate, 

5(2/3K20,  ViMgO),  12W03+24H20. 
Insol.  in  cold,   sol.  in  hot  H2O.      (Hallo- 
peau,  C.  R.  1898,  127.  621.) 

Magnesium    sodium    paratungstate,    3MgO, 

3Na2O,  14WO3+33H2O. 
Nearly   insol.   in   H2O.      (Knorre,    B.    19. 

825.) 

Manganous  tungstate,  MnWO4. 

Min.  Hubnerite.     Partially  sol.  in  HC1+ 

. 

+2H2O.  Insol.  in  H2O;  sol.  in  warm 
H3P04  and  H2C2O4+Aq;  si.  sol.  in  HC2H3O2 
+Aq.  Insol.  in  cold  HCl+Aq.  (Anthon.) 

+H2O.  Sol.  in  about  2500  pts.  H2O  at 
15°.  (Lefort.) 

Manganous  ^tungstate,  MnW2O7+3H2O  (?). 
Sol.  in  about  450  pts.  H2O  at  15°.  (Lefort, 
A.  ch.  (5)  15.  333.) 

Manganous  Zntungstate,  MnW3Oio+5H2O(?). 
Decomp.     by    H2O     into     MnW2O7     and 
MnW4O]3.    (Lefort,  A.  ch.  (5)  17.  480.) 

Manganous  metotungstate,  MnW4Oi3  + 

10H2O. 

Very  sol.  in  H2O.  (Wyrouboff,  Bull.  Soc. 
Min.  1892,  15.  82.) 

Manganous  paratungstate,  5MnO,  12WO3+ 
34H2O. 

(Gonzalez,  J.  pr.  (2)  36.  44.) 

Mn3W7O24+llH2O.  When  recently  pptd., 
sol.  in  a  small  amt.  of  H2O  acidulated  with 
HNO3.  (Lotz.) 

Manganous    potassium    tungstate,    2MnO, 

3K2O,  12WO3+16H2O. 
Completely    insol!    in    H2O.      (Hallopeau, 
Bull.  Soc.  1898,  (3)  19.  955.) 


TUNGSTATE,  POTASSIUM 


1093 


Manganous   sodium  paratungstate,   3Na2O, 

3MnO,  14W03+36H20. 
Sol.  in  H2O.    (Knorre,  B.  19.  826.) 

Manganic  sodium  tungstate. 
See  Permanganotungstate,  sodium. 

Mercurous  tungstate,  Hg2WO4. 

Insol.  in  H2O.     (Anthon.) 

Impossible  to  obtain  pure,  as  it  is  decomp. 
into — 

2Hg2O,  3WO3+8H2O.  Sol.  in  100  pts. 
H2O  at  15°.  (Lefort.) 

Mercurous  metatungstate.  Hg2W4Oi3-f- 

25H20. 
Ppt.    (Scheibler,  J.  pr.  83.  319.) 

Mercuric  tungstate,  HgWO4. 

SI.  sol.  in  H2O  and  very  unstable.    (Lefort, 

A.  ch.  (5)  15.  356.) 

3HgO,  2WO3.  Insol.  in  H2O.  (Anthon.) 
2HgO,  3WO3.  Insol.  in  H2O.  (Anthon.) 
3HgO,  5WO3+5H2O.  Sol.  in  about  250 

pts.  H2O  at  15°.     (Lefort.) 

2HgO,  5WO3+7H2O.    Decomp.  by  hot  or 

cold  H2O.    (Lefort,  C.  R.  88.  798.) 

Mercuric  Zntungstate,  HgW3O10+7H2O  (?). 

Sol.  in  about  120  pts.  H2O  at  15°.  (Lefort, 
A.  ch.  (5)  15.  360.) 

Molybdenum  tungstate. 

Easily  sol.  in  H2O.  Insol.  in  NH4Cl+Aq 
or  in  alcohol  of  0.87  sp.  gr.  (Berzelius.) 

Neodymium  tungstate,  Nd2(WO4)3. 

Very  si.  sol.  in  H2O.  1  pt.  is  sol.  in  52630 
pts.  H2O  at  22°;  59580  pts.  at  65°;  66040  pts. 
at  98°.  (Hitchcock,  J.  Am.  Chem.  Soc.  1895, 
17.  532.) 

Nickel  tungstate,  NiWO4. 

+3H2O.  Sol.  in  about  1000  pts.  H2O  at  15°. 
(Lefort.) 

+6H2O.  Insol.  in  H2O  or  H2C2O4+Aq. 
Sol.  in  boiling  H3PO4+Aq,  HC2H3O2+Aq,  or 
in  warm  NH4OH+Aq.  (Anthon.) 

Nickel  ^tungstate,  NiW2O7+5H2O  (?). 
Sol.  in  about  250  pts.  H2O.     (Lefort.) 

Nickel  ^ntungstate,  NiW3Oio+4H2O  (?). 

Sol.  in  H2O.  Pptd.  by  alcohol.  Decomp. 
by  cold  or  warm  H2O  after  above  pptn.  (Le- 
fort.) 

Nickel  wetatungstate,  NiW4O13+8H2O. 
Sol.  in  H2O.    (Scheibler,  J.  pr.  83.  273.) 

Nickel  paratungstate,  Ni3W7O24-fl4H2O. 

Insol.  in  H2O.  SI.  sol.  in  H2C2O4+Aq. 
Completely  sol.  in  warm  H3PO4  or  HC2H3O2-|- 
Aq.  (Anthon.) 


Potassium  tungstate,  K2WO4. 

Anhydrous.  Rather  deliquescent.  Easily 
sol.  in  H2O. 

+H2O.  Easily  sol.  in  H2O.  Insol.  in 
alcohol. 

+2H2O.  Very  sol.  in  H2O  with  absorption 
of  heat. 

1  pt.  dissolves  in  1.94  pts.  cold,  and  0.66 
pt.  boiling  H2O.  Alcohol  does  not  mix  with 
cone.  aq.  solution,  but  slowly  separates  out 
the  salt  from  it.  Acids,  even  H2SO3,  HC2H3O2 
or  H2C2O4,  separate  out  WO3  from  solution. 
(Riche,  A.  ch.  (3)  50.  45.) 

Potassium  ditungstate,  K2W2O7+2H2O. 

Sol.  in  about  8  pts.  H2O  at  15°,  but  on  heat- 
ing is  converted  into — 

+3H2O.  100  pts.  H2O  dissolve  only  2-3 
pts.  at  15°.  (Lefort,  A.  ch.  (5)  9.  102.) 

Potassium  ^n'tungstate,  K2W3O10+2H2O. 

Sol.  in  5-6  pts.  H2O  at  15°.  Can  be  re- 
cryst.  from  hot  H2O.  (Lefort,  A.  ch.  (5)  9. 
105.) 

Potassium  metatungstate,  K2W4Oi3+5H2O. 

Not  efflorescent.  Easily  sol.  in  H2O. 
(Marignac.) 

(K4W5Oi7+8H2O  of  Margueritte.) 
+8H2O.    Extremely  efflorescent.    (Scheib- 
ler.) 

Potassium  odotungstate,  K2W8O26. 

Insol.  in  H2O.     (Knorre,  J.  pr.  (2)  27.  49.) 

Potassium  tungstate,   K8Wi0O34+9H2O  = 
4K2O,  10WO3+9H2O. 

Properties  resemble  the  para  tungstate. 
(Gibbs,  Proc.  Am.  Acad.  16.  11.) 

+8H2O  =  K4W6O17-HH2O.  Sol.  in  15  pts. 
H2O  at  15°,  but  decomposed  by  heating  into 
K2W2O7  and  K2W3Oi0.  (Lefort,  A.  ch.  (5)  9. 
104.) 

Ki0WHO47.  Very  difficulty  sol.  in  cold, 
appreciably  sol.  in  hot  H2O,  probably  with 
decomposition.  (Knorre.) 

Potassium  paratungstate,  K10Wi2p4i+llH2O 
(or  K6W7O24+6H6O,  according  to  Lotz 
and  Scheibler.) 

Much  more  sol.  in  hot  than  cold  H2O.     (Anthon.) 
Sol.  in  100  pts.  H2O  at  16°,  in  8.5  pts.  at  100°.      (An- 

Sol.  in  46.5  pts.  cold,  and  15.15  pts.  boiling  EhO. 
(Riche.) 

By  shaking  the  crystals  several  days  at 
20°,  1  pt.  dissolves  in  71  pts.  H2O.  If  the 
salt  is  treated  with  boiling  water,  more  goes 
into  solution  the  Ipnger  it  is  boiled,  until 
after  several  days'  boiling  1  pt.  of  the  salt 
dissolved  in  5.52  pts.  H2O  at  18°.  Kept  in 
a  closed  flask,  this  solution  contained  after 
26  days  1  pt.  of  salt  to  11.9  pts.  H2O;  after 
153  days,  1  pt.  of  salt  to  15.6  pts.  H20;  after 
334  days,  1  pt.  of  salt  to  15.6  pts.  H2O.  In- 
sol. in  alcohol.  (Marignac.) 

+8H2O. 


1094 


TUNGSTATE,  POTASSIUM  SODIUM 


Potassium  sodium  tungstate,  K2WO4, 


Easily  sol.  in  hot  and  cold  H2O.  (Ullik, 
W.  A.  B.  66,  2.  150.) 

Deliquescent.  Sol.  in  1  pt.  cold,  and  YI  pt. 
hot  H2O.  (Anthon.) 

Potassium  sodium  paratungstate,  Na2O, 
4K20,  12WO3+15H2O. 

Sol.  in  H2O-.    (Marignac.) 

8/nNa2O,  3/nK2O,  12WO3+25H2O.  Sol.  in 
H2O.  (Marignac.) 

Potassium     strontium     tungstate     tungsten 

oxide,  5K2W4Oi2,  SrW4Oi2. 
(Engels,  Z.  anorg.  1903,  37.  143.) 

Potassium  uranous  tungstate. 
See  Uranosotungstate,  potassium. 

Potassium  zirconium  tungstate. 
See  Zirconotungstate,  potassium. 

Potassium  tungstate  tungsten  oxide,  K2WO4, 
W206. 

Potassium  tungsten  bronze.  (Scheibler,  J. 
pr.  83.  321.) 

Formula  is  K2W4Oi2.  Not  attacked  by 
acids,  and  only  very  si.  by  alkalies.  (Knorre, 
J.  pr.  (2)  27.  49.) 

K2WO4,  4WO2.  Not  attacked  by  acids, 
even  HF,  or  bv  alkalies +Aq.  Insol.  in 
alcohol.  (Zettnow,  Pogg,  130.  262.) 

Does  not  exist.    (Knorre.) 

Potassium  sodium  tungstate  tungsten  oxide, 
5K2W4Oi2+2Na4W6Oi5. 

Potassium  sodium  tungsten  bronze.  Prop- 
erties as  potassium  bronze. 

3K2W4Oi2,  2Na2W3O9.  As  above.  (Knorre, 
J.  pr.  (2)  27.  49.) 

Praseodymium  tungstate,  Pr2(WO4)3. 

Very  si.  sol.  in  H2O. 

Insol.  in  H2O  at  20°;  at  75°,  1  pt.  is  sol.  in 
23,300  pts.  H2O.  (Hitchcock,  J..Am.  Chem. 
Soc.  1895,  17.  529.) 

Rubidium  wetotungstate,  Rb2O,  4WO3  + 
8H20. 

Sol.  in  about  10  pts.  cold  H2O. 

Moderately  sol.  in  warm  H2O.  (Wyrou- 
boff,  Bull.  S6c.  Min.  1892,  15.  69.) 

Rubidium  pentotungstate,  Rb2W6O16. 

Almost  insol.  in  hot  H2O.  When  finely 
powdered,  it  is  sol.  in  alkali  carbonates +Aq. 
(Schaeffer,  Z.  anorg.  1904,  38.  163.) 

Rubidium  octotungstate,  Rb2W8O26. 

Insol.  in  H2O,  acids,  and  alkalies.  (Schaef- 
fer, Z  anorg.  1934,  38.  103.) 


Rubidium   paratungstate,    5Rb2O,   12WO3+ 

18H20. 

Very  si.  sol.  in  H2O.  (Schaeffer,  Z.  anorg. 
1904,  38.  173.) 

Samarium  metotungstate,   Sm2O3,   12WO3  + 
35H2O. 

Easily  sol.  in  H2O.    (Cleve.) 

Samarium  sodium  tungstate,  Na6Sm4(WO4)9. 
Insol.  in  H2O.     Slowly  sol.  in  dil.  acids, 
easily  in  cone.  HCl+Aq.     (Hogbom,   Bull. 
Soc.  (2)  42.  2.) 

Silver  (argentous)  tungstate,  Ag4O,  2WO3. 

HNOs+Aq  separates  WO3.  KOH+Aq 
dissolves  out  WO3  and  separates  Ag4O. 
(Wohler  and  Rautenberg,  A.  114.  120.) 

Does  not  exist.     (Muthmann,  B.  20.  983.) 

Silver  tungstate,  Ag2WO4. 

Sol.  in  about  2000  pts.  H2O  at  15°.  Easily 
decomp.  by  NaCl+Aq  or  BNO3+Aq. 
(Lefort.) 

Ag2W207.  Insol.  in  H2O.  Nearly  insol.  in 
HC2H302  or  H3PO4+Aq.  More  sol.  in 
KOH,  NH4OH+Aq,  or  H2C2O4+Aq.  (An- 
thon, J.  pr.  9.  347.) 

+H2O.  Sol.  in  about  5000  pts.  H2O  at 
15°.  (Lefort.) 

Silver  wetotungstate,  Ag2W4Oi3+3H2O. 
SI.  sol.  in  H2O.    (Scheibler,  J.  pr.  83.  318.) 
Nearly    insol.    in    H2O.      (Rosenheim,    Z. 

anorg.  1911,  69.  250.) 

Silver   paratungstate,   Ag10Wi2O4i+8H2O. 

(Gonzalez,  J.  pr.  (2)  36.  44.) 
Silver  tungstate  ammonia,  Ag2WO4,  4NH3. 

Sol.  in  H2O  with  rapid  decomp.  (Wid- 
mann,  Bull.  Soc.  (2)  20.  64.) 

Sodium  tungstate,  Na2WO4+2H2O. 

Sol.  in  4  pts.  cold,  and  2  pts.  boiling  H20. 
(Vauquelin  and  Hecht.) 

Sol.  in  1.1  pts.  cold,  and  0.5  pt.  boiling  H2O. 
(Anthon.) 

Sol.  in  2.44  pts.  H2O  at  0°;  1.81  pts.  at 
15°;  0.81  pt.  at  100°.  (Riche.) 

Solubility  in  H2O  at  t°. 


t 

%  Na2WOi 

Mols.  H2O 
to  1  mol. 
Na2WO4 

Mols.  of 
anhydrous 
salt  to 
100  mo  Is. 
H20 

-3.5 
+0.5 
21.0 
43.5 
80.5 
100.0 

41.67 
41.73 
42.27 
43.98 
47.65 
49.31 

22.87 

22.80 
22.30 
20.80 
17.95 
16.79 

4.37 
4.39 
4.48 
4.81 
5.57 
5.95 

(Funk,  B.  1900,  33.  3701.) 
See  also  -flOH2O. 

TUN  GST  ATE,  SODIUM 


1095 


Sp.  gr.  of  Na2WO4+Aq  at  24.5°  containing: 

Solubility  in  H2O  at  t°. 

5               10             15  %  Na2WO4+2H2O, 
1.036        1.075        1.119 

t° 

% 

Mols.  H2O 
to  1  mol 

Mols.  anhy- 
drous salt  to 

20             25             30  %  Na2WO4+2H2O, 

11  ftft           1    91  f»           1    97  d. 

Na2WO4 

Na2WO4 

100  mols.  H2O 

.1OO           1.Z1O           c.«f£ 

35             40             44  %  Na2WO4+2H2O. 

-5. 

30.60 

37.04 

2.70 

1.349        1.430        1.492 

—4.0 

31.87 

34.92 

2.86 

(Franz,  J.  pr.  (2)  4.  238.) 

-3.5 
-2.0 

32.98 
34.52 

33.19 
30.90 

3.01 
3.23 

0.0 

36.54 

28.37 

3.52 

+3.0 

39.20 

25.33 

3.95 

Sp.  gr.  of  Na2WO4+Aq  at  25°. 

+5.0 

41.02 

23.48 

4.26 

(Funk,  B. 

1900,  33.  3701.) 

Sp.  gr.  at  20° 

Per  cent  Na2WO4 

fer  cent 
a2        4,       2 

Sodium  rfituncstatc 

•NTn.W.0.. 

1.02016 

2.21 

2.48 

Sol.  in  H2O  by  heating  several  hours  to 

1.03915 

4.26 

4.78 

130-150°. 

(Knorre, 

J.  pr.  (2)  27.  80.) 

1.04292 

4.59 

5.15 

+6H2O 

Sol.  in  13  pts.  H2O 

at  15°.    (Le- 

1.05831 

6.25 

7.01 

fort,  C.  R. 

88.  798.) 

1.07449 

7.83 

8.79 

1.08209 
1.09687 
1.12114 
1  .  13036 
1.14392 
1  .  16896 
1.19154 

8.61 
10.08 
12.30 
13.16 
14.44 
16.56 
18.52 

9.66 
11.31 
13.81 
14.77 
16.21 
18.62 
20.79 

Sodium  Zntungstate,  Na2W3Oio+4H2O. 
Sol.  in  1  pt.  H2O.     Decomp.  on  standing 
into   sol.    tetratungst&te    and    insol.   cfo'tung- 
state.     (Lefort,  C.  R.  88.  798.) 
Neither  this  nor  the  other  fritungstates  of 
Lefort  exist,  according  to  Knorre  (J.  pr.  (2) 

1  .  19938 

19.10 

21.44 

27.  49.) 

1  .  20787 

19.74 

-22.16 

1.21720 

20.59 

23.11 

Sodium   wefatungstate,   Na2W4Oi3. 

1.25041 

23.16 

25.99 

Anhydrous.    Insol 

in  H2O. 

1.25083 

23.30 

26.15 

+10H2O.    Sol.  at 

13°.  in  0.935  pt.  H2O  to 

1.26234 

24.05 

27.00 

form  a  solution  of  3.02  sp.  gr.    (Scheibler.) 

1.28143 

25.46 

.       28.58 

Sol.  at  19°  in  0.195  pt.  H2O. 

(Forcher.) 

1.33993 

29.50 

33.11 

Precipitated  by  alcohol. 

1.38826 

32.68 

36.68 

1.41072 

33.91 

38.06 

Sodium  pentatungstate,  Na2W6Oi6. 

1.47193 
1.48481 
1.48595 

37.30 
38.20 
38.43 

41.87 
42.87 
43.14 

SI.  sol.  in  H2O  by  heating  3  hours  at  150°. 
(Knorre,  J.  pr.  (2)  27.  49.) 

C\  j«  j_.i^  _-.!.—  x—          "VT^    TIT  f\ 

(Pawlewski,  B.  1900,  33.  1224.) 


Na2WO4+Aq  is  pptd.  by  HC1,  HNO3,  or 
H2SO4+Aq,  but  not  by  H2SO3,  HI,  HCN, 
oxalic,  or  tartaric  acids +Aq,  but  pptn.  by  the 
former  acids  is  not  prevented  by  presence  of 
the  latter,  but  when  heated  with  HC2H3O2  + 
Aq,  or  in  presence  of  H3PO4+Aq,  mineral 
acids  cause  no  ppt.  (Zettnow,  Pogg,  130. 

-I  f*    \ 

Much  more  sol.  in  H2O2  than  in  H20. 
(Kellner,  Dissert,  1909.) 

SI.  sol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  829.) 

Insol.  in  alcohol.  (Riche,  A.  ch.  (3)  60. 
52  ) 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

+10H20. 


Insol.  in  H2O.  Very  difficultly  attacked 
by  acids  and  alkalies.  (Knorre.) 

+  12H2O.  Easily  sol.  in  cold  H2O,  and  can 
be  recryst.  without  decomp.  (Ullik,  W.  A.  B. 
66,  2.  157.) 

3Na2O,  8WO3+17H20.     Very  efflorescent. 

Very  sol.  in  hot  H2O.  (Wells,  J.  Am. 
Chem.  Soc.  1907,  29.  112.) 

Sodium  tungstate,  Na6W7O27  (?). 

+  16H2O  (?).  (Marignac,  A.  ch.  (3)  69. 
51.) 

+21H2O  (?).  Much  more  sol.  and  much 
more  rapidly  than  the  paratungstate.  (Ma- 
rignac.) 

Na4W3On+7H2O(?).  Mixture  of  Na2W4O13 
and  Na2WO4.  (Knorre,  J.  pr.  (2)  27.  49.) 

Na4W6Oi7  +  lLH2O.  Efflorescent.  Sol.  in 
H2O.  (Marignac.) 

100  pts.  H2O  dissolve  16  pts.  at  15°.  (Le- 
fort, A.  ch.  (5)  9.  97.) 

Formula  is  4Na2O,  10WO3+23H2O,  ac- 
cording to  Gibbs  (Proc.  Am.  Acad.  15.  5.) 


1096 


TUNGSTATE,  SODIUM 


Sodium  paratungstate,  Nai0Wi2O4i+21H2O. 

+25HoO. 

+28H2O  =  3Na6W7O24+ 16H2O.  according 
to  Lotz  and  Scheibler. 

Sol.  in  8  pts.  cold  H2O  (Anthon) ;  in  12.6  pts.  at  22°. 
(Forcher). 

Sol.  in  about  12  pts.  H2O.     (Marignac.) 
The  aqueous  solution  saturated  at  35-40° 
contained  to  1  pt.  of  the  salt,  after: 

1         12         77        227    410  days, 
at  18°       18°       18°       16°       20° 

9.25  11.26  10.92  11.90  11.74  pts.  H20. 

The  solution  saturated  by  very  long  boiling, 
after  a  part  of  the  salt  had  crystallised  out, 
contained,  after: 

1  2  12  days, 

0 . 68        0.91        2 . 59  pts.  H2O  to  1  pt.  salt, 

72  222          405  days, 

6 . 88        9 . 75      '  8 . 80  pts.  H2O  to  1  pt.  salt. 
(Marignac.) 

Decomp.  by  boiling  with"  H2O.  (Knorre, 
B.  18.  2362.) 

Sodium    strontium    paratungstate.    Na2O, 

4SrO,  12W03+29H20. 
(Gonzalez,  J.  pr.  (2)  36.  44.) 

Sodium  strontium  tungstate  tungsten  oxide. 
5NaW5O15,  SrW4012. 

12Na2W3O9,  SrW4O12.  (Engels,  Z.  anorg. 
1903,  37.  138.) 

Sodium  thorium  tungstate,  Na4Th(WO4)4. 

Insol.  in  H2O.  Slowly  sol.  in  dil.  acids, 
easily  in  cone.  HCl+Aq.  (Hogbom,  Bull. 
Soc.  (2)  42.  2.) 

Sodium  ytterbium  tungstate,  Yb203,  9Na2O, 
12WO3. 

Insol.  in  H2O.     (Cleve,  Z.  anorg.  1902,  32. 
154.) 
2Yb203,  4Na20,  7WO3.     Ppt.    '(Cleve.) 

Sodium  yttrium  tungstate,  Na8Y2(WO4)7. 

Insol.  in  H2O,  and  very  slowly  attacked  by 
dil.  acids.  (Hogbom,  Bull.  Soc.  (2)  42.  2.) 

Sodium  zinc  paratungstate,  Na2O,  2ZnO, 
7WO3+15H2O. 

Difficultly  sol.  in  cold,  more  sol.  in  hot  H2O 
(Knorre,  B.  19.  823.) 

+21H2O.     (Knorre.) 

Sodium  tungstate  tungsten  oxide,  Na2W04, 
W2O6. 

Yellow  tungsten  bronze.  Gradually  de- 
liquesces on  air.  Not  decomp.  by  any  acid, 
even  aqua  regia,  except  HF,  or  by  alkalies' 
(Wohler,  Pogg.  2.  350.) 

Correct  formula  is  NasWeOig.  according 
to  Phillip  (B.  16.  499). 


Sol.    in    ammoniacal   silver   solution   with 
separation    of    Ag.      Easily    sol.    in    boiling 
alkaline     potassium     ferricyanide-f  Aq. 
(Phillip,  B.  12.  2234.) 

Na2WO4,  2W2O6.  Blue  tungsten  bronze. 
Not  attacked  by  acids  or  alkalies.  (Scheibler.) 

Correct  formula  is  Na2W5Oi5,  according 
to  Phillip  (B.  16.  506). 

Sol.  in  ammoniacal  silver  solution  with 
separation  of  Ag. 

Na4W6Oi5.  Properties  as  above.  (Phillip, 
B.  16.  499.) 

Na2\fy3O9.    Properties  as  above.     (Phillip.) 

Strontium  tungstate,  SrWO4. 
Precipitate.     (Schultze.) 
Sol.  in  about  700  pts.  H2O.     (Lefort.) 

Strontium  ditungstate,  SrW2O7+3H2O  (?). 

100  ccm.  H2O  dissolve  0.35  g.  at  15°.  (Le- 
fort, A.  ch.  (5)  15.  326.) 

Strontium  ^ntungstate,  SrW3O10+5H2O  (?). 

Sol.  in  H2O  with  decomp.  into  SrW2O7  and 
SrW4Oi3.  (Lefort,  A.  ch.  (5)  17.  477.) 

Strontium  mefotungstate,  SrW4Oi3+8H2O. 

Solubility   as    calcium   meta tungstate. 
(Scheiblert) 

Extraordinarily  sol.  in  H2O.  (Wyrouboff, 
Bull.  Soc.  Min.  1892,  16.  63.) 

Strontium  paratungstate,  Sr3W7O24+16H2O, 

orSr5W12O41+27H2O. 
Insol.  in  cold,  si.  sol.  in  hot  H2O.    (Knorre, 
B.  18.  327.) 

Thallous  tungstate,  T12WO4. 

Very  si.  sol.  in  H2O.  Sol.  in  hot  Na2CO3+ 
Aq.  (Flemming,  J.  B.  1868.  250.) 

Thallous  raetatungstate,  T12W4O13+3H2O. 

Nearly  insol.  in  H2O.  (Rosenheim,  Z. 
anorg.  1911,  69.  251.) 

Thallous  paratungstate,  5T12O,  12WO3. 

Insol.  in  H2O. 

Sol.  in  Na2CO3+Aq.  and  K~OH+Aq. 
decomposed  bv  mineral  acids.  (Schaeffer,  Z. 
anorg.  1904,  38.  171.) 

Thallous  hydrogen  tungstate,  T1HWO4. 

Insol.  in  H2O.  Difficultly  sol.  in  NH4OH  + 
Aq.  Easily  sol.  in  boiling  alkali  carbonates 
or  hydrates  +Aq.  (Oettinger,  J.  B.  1864. 

^£)T:.  ) 

Thorium  tungstate. 

Precipitate.     (Berzelius.) 
Insol.  in  H2O. 

Tin  (stannous)  tungstate,  SnWO4+6H2O. 

Insol.  in  H2O.  Sol.  in  oxalic  acid  and  in 
KOH+Aq.  Slowly  sol.  in  hot  H3PO4+Aq. 
(Anthon,  J.  pr.  9.  341.) 


TUNGSTOCYANIDE,  MANGANOUS 


1097 


Tin  (stannic)  tungstate,  9SnO2,  13WO3. 

Insol.  in  ammonium  tungstate  -|-Aq.  Sol. 
in  tin  salts +Aq,  also  in  phosphoric,  oxalic, 
or  tartaric  acids +Aq.  (Lotz,  A.  91.  49.) 

Tungsten  tungstate,  WO2,  WO3  =  W2O5. 
See  Tungsten  oxide,  W2O5. 

Uranous  tungstate,  UO2,  3WO3+6H2O. 

Decomp.  by  NaOH+Aq  or  HNO3+Aq. 
Sol.  in  HCl+Aq,  but  not  in  H2SO4.  (Ram- 
melsberg.) 

Uranyl  tungstate,  UO3,  WO3+2H2O. 

Sol.  in  about  100  pts.  H2O.  (Lefort,  C.  R. 
87.  748.) 

UO3,  3WO3+5H2O  (?).  Sol.  in  about  200 
pts.  H2O.  (Lefort.) 

Vanadium  tungstate. 
SI.  sol.  in  H2O. 

Ytterbium  tungstate  basic,  (YbO)2WO4. 
Ppt.    (Cleve,  Z.  anorg.  1902,  32.  153.) 

Ytterbium  raetatungstate,   Yb2O3,    12WO3  + 

35H20. 
Very  sol.  in  H2O.    (Cleve.) 

Yttrium  tungstate,  Y2(WO4)3+6H2O. 

Very  si.  sol.  in  H2O,  but  more  sol.  in 
Na2WO4+Aq.  (Berlin.) 

Zinc  tungstate,  ZnWO4. 

Insol.  in  H2O.  (Geuther  and  Forsberg,  A. 
120.  270.) 

+H2O.    Sol.  in  503  pts.  H2O. 

Zinc  efttungstate,  ZnW2O7+3H2O  (?). 

Sol.  in  10  pts.  H2O  at  15°,  but  solution 
soon  decomposes.  (Lefort.) 

Zinc  in'tungstate,  ZnW3Oio+5H2O. 

Insol.  in  boiling  H2O.  Sol.  in  ZnSO4-f-Aq, 
or  Na4W6017+Aq.  (Gibbs.) 

Zinc  metatungstate,  ZnW4O13+10H2O. 

Easily  sol.  in  H2O.  Loses  crystal  H2O  by 
ignition,  and  becomes  insol.  in  H2O.  (Scheib- 
ler,  J.  pr.  83.  273.) 

-j-8H2O.  More  sol.  in  H2O  than  mag- 
nesium com  p.  (Wyrouboff,  Bull.  Soc.  Min. 
1892,  16.  72.) 

Zinc  tungstate,  Zn4W10O34+18H2O=4ZnO, 
10WO3+18H2O. 

Insol.  in  H2O.  Sol.  in  excess  of  zinc  sul- 
phate or  of  sodium  tungstate +Aq.  (Gibbs, 
Proc.  Am.  Acad.  15.  14.) 

+29H2O.     (Gibbs.) 

Zinc  paratungstate,  5ZnO,  12WO3-r-37H2O. 

(Gonzalez,  J.  pr.  (2)  36.  44.) 


Zinc   tungstate,    Zn9W22O76+66H2O=9ZnO, 

22WO3+66H2O.   . 
Insol.  in  H2O.     (Gibbs.) 

Zinc  tungstate  -ammonia,  ZnWO4,  4NH,+ 
3H2O. 

Decomp.  in  the  air.  (Briges,  Chem.  Soc. 
1904,  85.  677.) 

Pertungstic  acid. 
See  Pertungstic  acid. 

Tungstoarsenic  acid. 
See  Arseniotungstic  acid. 

Tungstoboric  acid. 
See  Borotungstic  acid. 

Tungstocyanhydric     acid,     H4W(CN)8+ 

Hydroscopic. 

Sol.  in  H2O  and  abs.  alcohol.  Insol.  in 
ether,  benzene  etc.  (Olsson.  Z.  anore.  1914, 
88.  71.) 

Ammonium  tungstocyanide,  (NH4)4W(CN)8. 

Easily  sol.  in  H2O.  Aqueous  solution  de- 
comp.  slowly. 

Insol.  in  organic  solvents.  (Olsson.  Z. 
anorg.  1914,  88.  62.) 

Cadmium     tungstocyanide,     Cd2W(CN)8-f- 

8H2O. 

Nearly  insol.  in  H2O.  SI.  sol.  in  dil.  HC1. 
Sol.  in  cone.  NH4OH-f  Aq.  Insol.  in  organic 
solvents.  (Olsson,  Z.  anorg.  1914,  88.  68.) 

Caesium  tungstocyanide,  Cs4W(CN)8. 

Easily  sol.  in  H2O  forming  stable  solutions. 
Insol.  in  alcohol  and  other  organic  solvents 

(Olsson.) 

Calcium  tungstocyanide,  Ca2W(CN)8-|-8H2O. 

Easily  sol.  in  H2O.  Aqueous  solution  de- 
comp.  slowly. 

Insol.  in  organic  solvents.    (Olsson.) 

Lead  tungstocyanide,  Pb2W(CN)8+4H2O. 

Sol.  in  H2O.  Solution  decomp.  after  short 
time. 

Insol.  in  organic  solvents.    (Olsson.) 

Magnesium  tungstocyanide,  Mg2W(CN)8-f 
6H20. 

Easily  sol.  in  H2O.  Aqueous  solution 
decomp.  on  heating. 

Insol.  in  organic  solvents.    (Olsson.) 

Manganous  tungstocyanide,   Mn2W(CN)8  + 


iganou 
8H2O. 


Insol.  in  H2O  and  in  acids. 

Insol.  in  organic  solvents.     (Olsson.) 


1098 


TUNGSTOCYANIDE,  POTASSIUM 


Potassium  tungstocyanide,  K4W(CN)8  + 
2H2O. 

Easily  sol.  in  H2O  from  which  it  can  be 
cryst.  10  ccm.  H2O  dissolve  13-14  g.  salt 
at  18°. 

Insol.  in  alcohol,  ether  and  other  organic 
solvents.  (Olsson.) 

Rubidium  tungstocyanide,  Rb4W(CN)8  + 
3H2O. 

Easily  sol.  in  H2O.    Can  be  cryst.  from  H2O. 

Insol.  in  alcohol  and  other  organic  solvents. 
(Olsson.) 

Silver  tungstocyanide,  Ag4W(CN)8. 
Insol.  in  H2O. 

Insol.  in  acids.    Decomp.  by  dil.  HC1. 
Sol.  in  hot  cone.  hH4OH+Aq. 
Insol.  in  organic  solvents.    (Olsson.) 

Sodium  tungstocyanide,   Na4W(CN)8+ 


Hydroscopic. 

Easily  sol.  in  H2O. 

Insol.  in  organic  solvents.     (Olsson.) 

Strontium  tungstocyanide,  Sr2W(CN)8+ 
8H2O,  +9H2O. 

Easily  sol.  in  H2O.  Aqueous  solution  de- 
comp.  on  standing. 

Insol.  in  organic  solvents.    (Olsson.) 

Thallium  tungstocyanide,  T14W(CN)8. 

Difficultly  sol.  in  cold  H2O,  more  sol.  in 
hot  H2O. 

Insol.  in  organic  solvents.    (Olsson.) 

Zinc  tungstocyanide,  Zn?W(CN)8+4H2O. 
Insol.  in  H2O,  and  acids. 
Sol.  in  cone.  NH4OH+Aq.    (Olsson.) 

Metotungstoiodic  acid. 

Ammonium  wetotungstoiodate, 

2(NH4)2O,  2I2O6,  4WO3+12H2O. 
Very  si.  sol.  in  H2O.     (Chretien,  A.  ch. 
5,  (7)  15.  431.) 


Potassium  tungstoiodate,  K2H3WIO8. 

(Blomstrand,  J.  pr.  (2)  40.  327.) 
2K2O,  2I2O6,  4WO3+8H2O. 
5.13  g.  are  sol.  in  1  1.  H2O  at  15°;  8.25  g. 
at  100°.    (Chretien,  A.  ch.  1898,  (7)  16.  431.) 

Tungstoperiodic  acid. 

Ammonium  sodium  tungstoperiodate, 

2(NH4)2O,  Na2O,  I207,  2WO3+16H2O. 
Ppt.    (Rosenheim,  A.  1899,  308.  64.) 

Barium  tungstoperiodate, 

5BaO,  I2O7,  12WO3+12H20. 
Ppt.    (Rosenheim.) 


Potassium  tungstoperiodate, 

5K2O,  I2O7,  12WO3+8H2O. 
Sol.  in  H2O.    (Rosenheim.) 

Sodium  tungstoperiodate, 

3Na2O,    I2O7,    2WO3+4H2O. 

Ppt. 

5Na2O.  I2O7,  12WO3+16H2O.  Sol.  in 
H2O.  (Rosenheim.) 

Strontium  tungstoperiodate, 

5SrO,  I207,  12W03+28H20. 
Sol.  in  H2O.     (Rosenheim.) 

Tungstophosphoric  acid, 
See  Phosphotungstic  acid. 

Tungstosilicic  acid, 
See  Silicotungstic  acid. 

Tungstotungstic  acid. 

Lithium     tungstotungstate,     Li2O,     WO8+ 

WO2,  3WO3. 

Insol.  in  boiling  H2O  and  cone.  HC1. 
(Hallopeau,  C.  R.  1898,  127.  514.) 

Potassium    tungstotungstate,    K2O,    WO3+ 

W02,  3W03. 

Insol.  in  hot  H2O,  and  cone.  HC1.  (Hallo- 
peau, Bull.  Soc.  1899,  (3)  21.  267.) 

Tungstous  acid. 

Sodium  tungstite,  Na2W205. 
See  Tungstate  tungsten  oxide,  sodium. 

Tungstovanadic  acid. 
See  Vanadiotungstic  acid. 

Tungstyl  dibromide,  WO2Br2. 

Not  decomp.  by  cold  H2O.    (Roscoe.) 

Tungstyl  ^rabromide,  WOBr4. 

Extremely  deliquescent.  Decomposes  at 
once  in  moist  air  or  with  H2O. 

Tungstyl  bichloride,  WO2C12. 

Not  decomp.  by  cold,  and  but  slowly  by 
boiling  H2O..  Sol.  in  alkalies  and  ammonia. 

Tungstyl  ^rachloride,  WOC14. 

Easily  decomp.  by  H2O  or  moist  air. 

Very  sol.  in  CS2  and  S2C12.  SI.  sol.  in  ben- 
zene. (Smith,  J.  Am.  Chem.  Soc.  1899,  21. 
1008.) 

Tungstyl  ^rafluoride,  WOF4. 

Sol.  in  H2O  with  decomp.  Very  hydro- 
scopic. 

Insol.  in  carbon  tetrachloride. 


URANATE,  POTASSIUM 


1099 


SI.  sol.  in  carbon  bisulphide,  dry  benzene 
and  ether. 

Easily  sol.  in  chloroform  and  absolute 
alcohol.  (Ruff,  Z.  anorg.  1907,  62.  265.) 

Tungstyl   teirafluoride  ammonia,   2WOF4, 
NH3. 

Sol.  in  H2O  with  decomp. 
Insol.   in   liquid   NH3.      (Ruff,   Z.   anorg 
1907,  52.  266,) 

Ultramarine  blue,  2Na2Al2Si2O8,  Na2S2  (?) 
Not  attacked  by  solutions  of  alkalies  or 
NH4OH+Aq.      Decomp.   by   acids   or  acid 
salts  +Aq.    Decomp.  by  alum+Aq. 

Ultramarine  green,  Na2Al2Si2O8,   Na2S  (?). 

Decomp.  by  mineral  aqids.  Not  attacked 
by  alkalies.  Decomp.  by  alum  +Aq. 

Ultramarine  white,  2Na2Al2Si2O8,  Na2S  (?). 

Uranic  acid,  H2UO4. 

Insol.  in  H2O.  Sol.  in  acids.  Very  sol.  in 
cold  dil.  HNO3+Aq.  SI.  sol.  in  boiling 
NH4Cl+Aq.  Insol.  in  KOH,  NaOH,  or 
NH4OH+Aq.  Easily  sol.  in  (NH4)2CO3, 
KHCO3,  and  NaHCO3+Aq;  less  in  K2CO3  + 
Aq.  (Ebelmen.) 

Easily  sol.  in  malic  and  tartaric  acids  to 
form  complex  compds.  (Itzisr,  B.  1901,  34. 
3822.) 

H4UO5.  Insol.  in  H2O;  sol.  in  acids. 
(Ebelmen.) 

Uranates. 

Insol.  in  H2O;  sol.  in  acids. 

Ammonium  uranate. 

SI.  sol.  in  pure  H2O;  insol.  in  H2O  contain- 
ing NH4C1  or  NH4OH. 

Sol.  in  (NH4)2CO3+Aq.  (Peligot,  A.  ch. 
(3)  6.  11.) 

(NH4)2O,  4UO3+7H2O.  (Grubler,  Dis- 
sert, 1908.) 

(NH4)2O,  6UO3  +  10H2O.  Insol.  in  cold 
and  hot  H2O  and  alkalies +Aq.  Very  sol.  in 
H2SO4,  HC1  and  acetic  acid  +Aq.  (Zehenter, 
M.  1900,  21.  235.) 

Barium  uranate,  BaU04. 

Insol.  in  H2O.    Sol.  in  dil.  acids. 

BaU2O7.    As  above.    (Ditte,  C.  R.  95.  988.) 

BaU3Oio+4^H2O.  Nearly  insol.  in  H2O, 
KOH+Aq.  and  alcohol. 

Easily  sol.  in  cold  dil.  HC1  or  HNO3  and  in 
hot  acetic  acid.  (Zehenter,  M.  1904,  26.  200.) 

Ba2U6Oi7+8H2O.  Nearly  insol.  in  hot 
or  cold  H2O,  KOH+Aq.  and  alcohol. 

Easily  sol,  in  cold  dil.  HC1  or  HNO3  and  in 
hot  acetic  acid.  (Zehenter.) 

Ba2U7O23  +  llH2O.  Same  properties  as 
BaU3O10.  (Zehenter.) 


Bismuth  uranate,  Bi2O3,  UO3-f-H2O. 
Min.   Uranosphaerite. 

Calcium  uranate,  CaUO4. 

Insol.  in  H2O;  sol.  in  dil.  acids.  (Ditte, 
C.  R.  96.  988.) 

CaU2O7.     Insol.  in  H2O;  sol.  in  dil.  acids 

(Ditte.) 

Cobalt  uranate. 

Insol.  in  H2O;  sol.  in  Pb(C2H3O2)2-|-Aq. 
(Persoz,  J.  pr.  3.  216.) 

Sol.  in  HNO3+Aq;  insol.  in  KNO3+Aq. 
(Ebelmen,  A.  ch.  (3)  5.  222.) 

Cupric  uranate,  CuU2O7. 

Insol.  in  H2O.    (Debray,  A.  ch.  (3)  61.  451.) 

Lead  uranate,  PbUO4. 

If  ignited,  very  difficultly  sol.  in  HC2H3O2  + 
Aq.  (Wertheim,  J.  pr.  29.  228.) 

Insol.     in     Pb(C2H3O2)2+Aq.       (Persoz.) 
3PbO,    2UO3.      Sol.    in    dil.    HNO3+Aq. 
(Ditte,  A.  ch.  (6)  1.  338.) 
PbU3Oio.     Insol.  in  H2O.     Sol.  in  HNO3 
Insol.    in   KOH+Aq,    NH4OH   and    cold 
acetic  acid.    Sol.  in  hot  acetic  acid.    (Zehen- 
ter, M.  1904,  25.  215.) 

Pb4U6O19+4H2O.  Insol.  in  hot  or  cold 
H2O.  Sol.  in  HNO3.  Insol.  in  KOH+Aq, 
NH4OH,  alcohol  and  ether.  SI.  sol.  in  cola, 
more  easily  sol.  in  hot  acetic  acid.  (Zehenter.) 

Lithium  uranate,  Li2UO4. 

Insol.  in  H2O',  but  decomp.  thereby.  Sol. 
n  dil.  acids. 

Magnesium  uranate,  MgUO4. 

Insol.  in  H2O.  Nearly  insol.  in  cold  HC1  + 
Aq.  Slowly  sol.  in  HCl+Aq  on  warming, 
and  more  rapidly  by  addition  of  a  little  HNO3 
+Aq.  (Ditte.) 

MgU2O7.    Ppt.     (Berzelius.) 

Neodymium  uranate,  Nd2(U3Oio)3+18H2O. 
Ppt.     (Orloff,  Ch.  Z.  1907',  31.  1119.) 

Potassium  uranate,  K2UO4  (?). 

Insol.  in  H2O;  sol.  in  dil.  acids,  etc.,  exactly 
as  Na2UO4.  (Ditte.) 

K2U2O7+6H2O.  Insol.  in  H2O.  Sol.  in 
dil.  acids,  even  acetic  acid.  (Zimmermann, 
B.  14.  440.) 

Insol.  in  K2CO3+Aq.  but  easily  sol.  in 
alkali  hydrogen  carbonates +Aq.  Sol.  in 
HCl+Aq.  (Ebelmen,  A.  ch.  (3)  6.  220.) 

K2O,  4UO3+5H2O.  (Zehenter,  M.  1900, 
21.  235.) 

K2O,  6UO3+6H2O.  Insol..  in  H2O. 
Drenckmann,  Zeit.  ges.  Nat.  17.  113.) 

+  10H2O.  Nearly  insol.  in  cold  and  hot 
:E2O.  Easily  sol.  in  hot  acetic  acid,  dil.  H2SO4 
HC1  and  HNO3.  Insol.  in  KOH+Aq,  alco- 
10!  and  ether.  ((Zehenter,  M.  1900,  21.  235.) 


1100 


URANATE,  POTASSIUM  HYDROXYLAMINE 


Potassium  hydroxylamine  uranate, 

UO4(NH4O)(NH3OK)  +H2O. 
SI.  sol.  in  H2O ;  insol.  in  alcohol.    (Hofmann, 
A.  1899,  307.  318.) 

Rubidium  uranate,  RbUO4. 

Insol.  in  H2O.     (Ditte,.  A.  ch.  (6)  1.  338.) 

Silver  uranate,  Ag2U2O7. 

Insol.  in  H2O.  Easily  sol.  in  acids.  (Alibe- 
goff,  A.  233.  117.) 

Sodium  uranate,  Na2UO4  (?). 

Insol.  in  H2O;  sol.  in  dil.  acids.  Sol.  in 
alkali  carbonates +Aq.  (Ditte.) 

Na2U2O7+6H2O.  Insol.  in  H2O.  Sol.  in 
dil.  acids.  (Stolba,  Z.  anal.  3.  74.) 

Na2O,  3UO3.  Insol.  in  H20.  Easily  sol.  in 
very  dil.  acids.  (Drenckmann.) 

Na2O,  5UO3+5H2O.  Insol.  in  H2O,  alco- 
hol, NH4OH.  KOH+Aq.  Sol.  in  HC1,  HNO3, 
H2SO4.  SI.  sol.  even  on  boiling  in  cone, 
acetic  acid.  (Zehenter,  M.  1900,  21.  235.) 

Sodium  hydroxylamine  uranate, 

UO4(NH4O)(NH3ONa)  +H2O. 
Sol.  in  H2O.    (Hofmann,  A.  1899,  307.  319.) 
UO4(NH3ONa)2+6H2O.    Very  sol.  in  H2O. 

(Hofmann.) 

Strontium  uranate,  SrUO4. 

Insol.  in  H2O.    Sol.  in  dil.  acids. 

SrU2O7.    As  above.    (Ditte,  C.  R.  96.  988.) 

Very  si.  sol.  in  H2O.  Sol.  in  all  acids 
especially  oxalic. 

+H2O.  Very  si.  sol.  in  H2O.  Sol.  in  all 
acids  especially  oxalic.  (J,  C.  C.  1896,  II. 
512.) 

Thallous  uranate. 

Ppt.  (Bolton,  Am.  Chemist,  1872,  2. 
456.) 

Zinc  uranate. 

Insol.  in  H2O;  sol.  in  Pb(C2H3O2)2+Aq. 
(Persoz,  J.  pr.  3.  216.)  Sol.  in  HNO3+Aq; 
insol.  in  KNO3,  and  NH4NO3+Aq.  (Ebel- 
men.  A.  ch.  (3)6.221.) 

Pmiranic  acid. 
See  Peruranic  acid. 

Uranium,  U. 

Not  attacked  by  H2O.  Slowly  decomp.  by 
cold  dil.  H2SO4+Aq,  rapidly  on  warming. 
Easily  sol.  in  dil.  or  cone.  HCl+Aq.  Fused 
U  is  slightly  attacked  by  cone,  or  fuming 
HNO3,  or  cone.  H2SO4.  Amorphous  U,  how- 
ever, is  easily  attacked  thereby.  Not  at- 
tacked by  acetic  acid,  KOH,  NaOH,  or 
NH4OH+Aq.  (Zimmermann,  B.  16.  849.) 

When  finely  divided,  it  is  decomp.  by  H2O 
slowly  at  ordinary  temps,  and  rapidly  at 
100°.  (Moissan,  C.  R.  1896,  122.  1091.) 


Uranium  antimonide,  U3Sb2. 

Violently  attacked  by  cone.  HNO3.  (Co- 
lani,  C.  R.  1903,  137.  383.) 

Uranium  arsenide,  U3As2. 

Violently  attacked  by  cone.  HNO3.  (Co- 
ani,  C.  R.  1903  137.  383.) 

Uranium  boride,  UB2. 

Sol.  in  HNO3  and  HF.  Deiomp.  by  fused 
alkalies.  (Wedekind,  B.  1913,  46.  1204.) 

Uranium  ^n'bromide,  UBr3. 

Very  hygroscopic.  Sol.  in  H2O  with  hiss- 
ing. (Alibegoff,  A.  233.  117.) 

Uranium  te£rabromide,  UBr4. 

Anhydrous.  Very  deliquescent.  Sol.  in 
H2O  with  hissing.  (Hermann.) 

Insol.  in  alcohol,  (v.  Unruh,  Dissert,  1909.) 

Sol.  in  acetone.  (Eidmann.  C.  C.  1899,  II. 
1014);  methyl  acetate  (Naumann,  B.  1909, 
42.  3790);  ethyl  acetate.  (Naumann,  B. 
1904,  37.  3601.) 

+8H2O.  Very  deliquescent,  and  sol.  in 
H.O.  (Rammelsberg.) 

Uranium  carbide,  UC2. 

(Ruff  and  Heinzelmann,  Z.  anorg.  1911, 
71.  72.) 

Attacked  slowly  by  H2O.  Slowly  attacked 
by  cold  dil.  HC1,  H2SO4  or  HNO3+Aq. 
Cone,  acids,  except  HNO3,  react  si.  in  the 
cold,  violently  on  heating.  (Moissan,  Bull. 
Soc.  1897,  (3)  17.  12.) 

Sol.  in  fused  KNO3  and  KC1O3;  sol.  in  dil. 
acids  in  the  cold  and  in  cone,  acids  on  heating; 
decomp.  by  H2O.  (Moissan,  C.  R.  1896, 
122.  276.) 

Uranium  /nchloride,  UC13. 
Very  sol.  in  H2O.     (Peligot.) 
Very  unstable.     (Zimmermann.) 
Very  hygroscopic.     Sol.  in  H2O  with  de- 
comp.    Sol.   in   cone.    HC1   and   solution   is 
much  more  stable  than  aqueous  one.    (Rosen- 
heim  and  Loebel,  Z.  anorg.   1908,  57.  234.) 

Uranium    te^rachloride,    UC14. 

Anhydrous.     Extremely  deliquescent. 

Sol.  in  H2O  with  evolution  of  heat.  De- 
comp. on  boiling.  Sol.  in  NH4Cl+Aq  with- 
out decomp. 

HC1  increases  its  solubility  in  H2O.  (Aloy, 
Dissert.  1901.) 

Sol.  in  alcohol,  acetone,  acetic  ether,  ben- 
zoic  ether.  Insol.  in  ether,  CHC1  and 
C6H6.  (Loebel.) 

Sol.  in  ethyl  acetate.  (Naumann,  B.  1904, 
37.  3601.) 

Uranium  pentochloride,  UC15. 

Deliquescent.  Sol.  in  H2O  with  evolution 
of  heat  and  decomposition.  .Roscoe,  B.  7. 
1131.) 


URANOURANIC  OXIDE 


1101 


Sol.  in  acetic  acid,  acetic  ether,  benzalde- 
hyde,  glycerine,  benzyl  alcohol  (trace), 
nitrobenzene  (trace),  xylidine  and  p-toluidine 
(on  warming). 

Insol.  in  aniline,  ligroin,  pyridine,  quinoline, 
thioethyl  ether,  thioamyi  ether  and  CS2 
(Pimmer,  Dissert.  1904.) 

Sol.  in  abs.  alcohol.  Insol.  in  ether,  C6H6, 
nitrobenzene,  ethylene  bromide.  SI.  sol. 
in  CC14  and  CHC13.  Sol.  in  benzoic  ethsr, 
acetone  and  trichloracetic  acid.  Best  solvents 
are  ethyl  acetate  and  benzonitrile.  Sol.  in 
many  organic  compounds  containing  oxygen. 
(Loebel,  Dissert.  1907.) 

Uranium  ^'fluoride,  UF2+2H2O. 

Ppt  (Giolitti  and  Agamennone,  C.  C. 
1905,  I.  1130.) 

Uranium  tefrafluoride,  UF4. 

Insol.  in  H2O.  Very  si.  sol.  in  dil.  acids. 
Sol.  in  hot  cone.  HaSO-t,  and  slowly  in  warm 
cone.  HNO3+Aq.  (Bolton,  J.  B.  1866.  209.) 

Uranium  Aezafluoride,  UF6. 

Very  sol.  in  H2O.  (Ditte,  A.  ch.  (6)  1. 
339.) 

Fumes  in  the  air. 

Very  hydros^opic;  sol.  in  H2O.  (Ruff,  B. 
1909,  42/495.) 

Very  hygrosoopic.  Sol.  in  H2O.  Nearly 
insol.  in  CS2.  Insol.  in  paraffine  oil.  Sol.  in 
symmetrical  tetrachlorethane  (best  solvent), 
CHC13,  CC14,  and  nitrobenzene,  (v.  Unruh, 
Dissert.  1909.) 

Decomp  v    by    H2O,    alcohol    and    ether. 

Nearly  insol.  in  CS2. 

Sol.  in  CHC13,  CC14,  nit  obenzene  and 
C2H2C14.  (Ruff,  Z.  anorg.  1911,  72.  81.) 

Uranium  hydrogen  fluoride,  UF6,  8HF  (?). 
Sol.  in  H2O.     (Ditte.) 
Is  U02F2,  HF+H20.    (SmitheUs  ) 

Uranous  hydroxide,  UO2,  zH2O. 

Easily  sol.  in  dil.  acids. 

Insol.  in  alkali  hydrates  and  carbonates 
+Aq.  (Berzelius.) 

Sol.  in  alkali  carbonates +Aq.  (Rammels- 
berg.) 

U(OH)4.  Sol.  in  dil.  acids.  (Aloy,  Bull. 
Soc.  1899,  (3)  21.  613.) 

Uranouranic  hydroxide,  U3O8,  6H2O  (?). 

Easily  sol.  in  acids. 

Decomp.  by  (NH4)2CO3+Aq,  which  dis- 
solves out  UO3.  (Berzelius.) 

Uranic  hydroxide. 
See  Uranic  acid. 

Uranium  te^raiodide,  UI4. 

Sol.  in  H2O.  (Guichard,  C.  R.  1907,  145. 
921.) 


Uranium  iodide. 

Sol.  in  ethyl  acetate..  (Naumann.  B.  1904 
37.  3601.) 

Uranium  nitride,  U3N4. 

(Colani,  C.  R.  1903.  137.  383.) 

Uranium  sw&oxide,  UO  (?). 

(Guyard,  Bull.  Soc.  (2)  1.  89.) 

Does  not  exist.  (Zimmermann,  A.  213. 
301.) 

U2O3(?).  Ppt.  Decomp.  by  H20  and  in 
the  air.  (Peligot.) 

Uranium  dioxide  (Uranous  oxide),  UO2. 

Insol.  in  dil.  HC1  or  H2SO4+Aq. 

Sol.  in  cone.  H2SO4,  and  easily  in  HNO3+ 
Aq.  (Peligot.) 

Insol.  in  NH4Cl+Aq.     (Rose.) 

Only  si.  sol.  in  H2SO4,  but  a  considerable 
amount  is  converted  into  the  sulphate  which 
is  nearly  insol.  in  H2SO4. 

Slowly  sol.  in  HC1,  the  amount  dissolved 
in  a  given  time  varying  widely  with  the 
method  of  preparation  of  the  oxide.  (Colani, 
C.  R.  1912,,  155.  1251.) 

SI.  more  sol.  in  HNO3  than  in  aqua  regia. 
(Raynaud,  Bull.  Soc.  1912,  (4)  11.  802.) 

Very  sol.  in  cone.  HNO3;  less  sol.  in  dil. 
HNO3.  1  gram  is  sol.  in  3100  grams  HC1 
(1.17)  at  17°;  4650  grams  HBr(1.52)  at  17°; 
2200  grams  H2SO4(1.79)  at  17°;  12,000  grams 
acetic  acid  at  19°.  (Raynaud,  C.  R.  1911, 
153.  1481.) 

SI.  attacked  by  liquid  NH3.  (Gore,  Am. 
Ch.  J.  1898,  20.  830.) 

Min.  Uraninite.  Easily  sol.  in  warm 
HNO3+Aq.  Not  attacked  V  HCl+Aq. 

Uranium  dioxide  (Uranic  oxide),  UO3. 

Sol.  in  HNO3+Aq.     (Peligot.) 

Insol.  in  boiling  K  tartrate  +Aq.  (Kah- 
lenberg  and  Hijlyer,  Am.  Ch.  J.  1894, 16.  102.) 

Sol.  in  oleic  acid.  (Gibbons,  Arch.  Pharm. 
1883,  221.  621.) 

See  Uranic  acid. 

Uranium  te.!roxide,  UO4. 

Decomp.  by  HCl+Aq.  (Fairley,  Chem. 
Soc.  31.  133.) 

-f  2H2O.  •  Very  hygroscopic.  (Zimmer- 
mann.) 

+3H2O. 

Uranium  pentoxide,  U2O6. 

Sol.  in  acids.     (Peligot.) 

Mixture  of  UO3  and  U3O8.  (Ramrnels- 
berg,  Pogg.  59.  5.) 

Mixture  of  UO2  and  U3O8.  (Zimmermann, 
A.  232.  273.) 

Uranouranic  oxide,  U3O8. 

Green  uranium  oxide.  Very  slowly  and 
slightly  sol.  in  dil.  HC1  or  H2SO4+Aq;  more 
easily  when  cone.  Completely  sol.  in  boil- 
ing H2SO4.  Easily  sol.  in  HNO3+Aq. 


1102 


URANOUS  OXYCHLORIDE 


Uranous  oxychloride,  U02,  UC14+H2O. 

Moderately  sol.  in  H2O.     (Aloy,  Dissert. 
1901.) 

2U02,  UC14+H20.  Very  sol.  in  H20 
and  alcohol.  (Orloff,  C.  C.  1903,  II.  484.; 

+  13H2O.  Very  sol.  in  H2O  and  alcohol 
(Orloff.) 

4UO2,  UC14.  Very  sol.  in  H2O  and  alcohol 
(Orloff.) 

5UO2,  UC14  +  10H2O.  Insol.  in  H2O 
(Aloy,  Dissert,  1901.)  • 

Uranous  oxyfluoride,  UOF2+2H2O. 

(Giolitti  and  Agamennone,  C.  C.  1905,  I 
1130.) 

Uranous  oxysulphide,  U3O2S4=U02,  2US2. 

Slightly  attacked  by  dil.,  easily  by  cone. 
HCl+Aq.  Sol.  in  cold  HNO3+Aq.  (Her- 
mann, J.  B.  1861.  258.) 

Uranic  oxy-compounds. 
See  Uranyl  compounds. 

Uranium  phosphide,  U3P2. 

Violently  attacked  by  cone.  HNO3. 
(Colani,  C.  R.  1903,  137.  383.) 

U3P4.     Slowly  attacked  by  H2O,  not  by 
dil.    HCl+Aq.      More    easily    attacked    by 
cone.  HCl+Aq.     Quickly  decomp.  by  boil- 
ing cone.  HNO3  and  HNOs+HCl.     (Colani, 
A.  ch.  1907,  (8)  12.  59.) 

Uranium  selenide,  USe. 

Spontaneously  inflammable.     Sol.  in  fum- 
ing HNO3.     (Colani.  C.  R.  1903,  137.  383.) 
USe2.     As  US2.     (Colani.  C.  C.  1903,  II. 

707.) 

U2Se3.     (Colani.) 

Uranium  cKsilicide,  USi2. 

Sol.  in  cold  or  hot  cone.  HF;  insol.  in  HC1, 
HNO3,  H2SO4  and  aqua  regia.  (Defacqz, 
C.  R.  1908,  147.  1051.) 

Uranium  monosulphide,  US. 
(Alibegoff,  A.  233.  117.) 

Uranium  sesgwsulphide,  U2S3. 

Not  attacked  by  HC1  or  dil.  HNO3+Aq. 
Oxidised  by  fuming  H2SO4  or  aqua  regia. 
(Alibegoff,  A.  233.  117.) 

Uranium  cfo'sulphide,  US2. 

Insol.  in  cold  or  boiling  dil.  HCl+Aq. 
Sol.  in  cold  cone.  HCl+Aq.  Decomp.  by 
HNO3+Aq.  (Hermann.  J.  B.  1861.  258.) 

Uranium  telluride,  U4Te3. 

Violently  attacked  by  cone.  HNO3. 
(Colani,  C.  R.  1903,  137.  383.) 


Uranosotungstic  acid. 

Potassium  uranosotungstate,   9K2O,    6UO2, 

8WO3+34H2O. 

Insol.  in  H2O  and  in  HC1.     (Gibbs,  Am. 
Ch.  J.  1895,  17.  175.) 

Sodium   uranosotungstate,    12Na2O,    6U02, 

8WO3+25H2O. 
Insol.  in  cold  H2O.     (Gibbs.) 

Uranyl  bromide,  UO2Br2. 
Sol.  in  H2O.     (de  Coninck,  C.  C.  1903,  I. 

693.) 

Sol.  in  ether,     (v.  Unruh,  Dissert.  1909.) 
+7H2O.     Deliquescent.     Sol.  in  H2O. 

Uranyl  bromide  ammonia,  UO2Br2,  2NH8. 
(v.  Unruh,  Dissert.  1909.) 
UO2Br2,  3NH3.     (v.  Unruh.) 
UO2Br2,  4NH3.    (v.  Unruh.) 

Uranyl  chloride,  UO2C12. 

Anhydrous.     Very   deliquescent.      Sol.    in 
H2O,  alcohol,  and  ether. 
Very  sol.  in  H2O. 

Sp.  gr.  of  UO2Cl2+Aq  at  t°. 


t° 

%  U02C12 

Sp.  gr. 

14.6 

1 

1.0056 

16.3 

2 

1.0112 

13.7 

3 

1.0161 

13.1 

4 

1.0215 

14.2 

5 

1.0260 

15.2 

6 

1.0313 

14.3 

7 

1.0366 

14.5 

8 

1.0418 

15.0 

9 

1.0469 

14.8 

10 

1.0517 

(de  Coninck,  A.  ch.  1904,  (8)  3.  500.) 

Sol.  in  cone.  HC1,  cone.  HNO3  and  in 
selenic  acid. 

Decomp.  by  H2SO4.  (de  Coninck.  A.  ch. 
1904,  (8)  3.  504.) 

Sol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790) ;  acetone.  (Naumann,  B.  1904, 
37.  4328.) 

+H2O.     Sol.  in  H2O,  alcohol,  and  ether. 

+3H2O.     Deliquescent. 

Very  sol.  in  H2O.  1  pt.  is  sol.  in  0.134  pts. 
H2O  at  18°  and  solution,  which  is  saturated, 
contains  76.2%  UO2C12  or  88.2%  UO2C12  + 
3H2O.  Sp.  gr.  of  solution  =  2.740.  The 
solubility  increases  with  rise  in  temp. 

Sol.  in  alcohol  and  in  ether.  (Mylius  and 
Dietz,  B.  1901,  34.  2775.) 

Uranyl  hydrogen  chloride,.  UO2C12,   HC1+ 
2H2O. 

Cryst.  at  -  10°  from  sat.  solution  of  UO2C12 
n  HCl+Aq. 


VANADATE,  AMMONIUM 


1103 


Fumes  in  the  air.     (Aloy,  Bull.  Soc.  1901, 
(3)  25.  154.) 


Uranyl  chloride  ammonia,  U02(NH3C1)2. 

Decomp.  by  H2O.  (Regelsberger,  A.  227. 
119.) 

UO2(NH3.NH3C1)NH3C1.  Decomp.  by 
H2O.  (Regelsberger.) 

UO2(NH3.NH3C1)2.  Decomp.  by  H2O. 
(Regelsberger.) 

Uranyl  fluoride,  UO2F2. 

Very  sol.  in  H2O.  (Smithells,  Chem.  Soc. 
43.  125.) 

Insol.  in  H2O  or  dil.  acids.  Very  si.  sol.  in 
HF+Aq.  Sol.inH2SO4+aquaregia.  (Ditte, 
A.  ch.  (6)  1.  339.) 

Insol.  in  ether  and  amyl  alcohol.  (v. 
Unruh,  Dissert,  1909.) 

UOF4.  Very  sol.  in  H2O.  (Ditte,  C.  R. 
91.  115.) 

True  composition  is  U02F2.     (Smithells.) 

Uranyl  hydrogen  fluoride,  UO2F2,  HF+H2O. 

Very  sol.  in  H2O.  (Smithells,  Chem.  Soc. 
43.  131.) 

Uranyl  fluoride  ammonia,  UO2F2,  2NH8. 
(v.  Unruh,  Dissert.  1909.) 
UO2F2,  3NH3.     (v.  Unruh.) 
UO2F2,  4NH3.     (v.  Unruh.) 

Uranyl  iodide,  UO2I2. 

Ppt.  Deliquescent.  (Aloy,  A.  ch.  1910, 
(7)  24.  417.) 

Deliquescent. 

Sol.  in  alcohol,  ether  and  benzene.  (Aloy, 
Dissert.  1901.)  -  uy 

Sol.  in  acetone.  (Eidmann,  C.  C.  1899,  II. 
1014;  Naumann,  B.  1904,  37.  4328);  methyl 
acetate.  (Naumann,  B.  1909,  42.  3790.) 

Uranyl  iodide  ammonia,  U02I2,  2NH3. 
(Aloy,  Dissert.  1901.) 
UO2I2,  3NH3.     (Aloy.) 
UO2I2,  4NH3.     (Aloy.) 

Uranyl  selenide,  UO2Se. 

Very  slowly  decomp.  by  H2O. 

Easily  sol.  in  cold  HC1.  Violently  attacked 
by  cold  HNO3.  Not  attacked  by  dil.  alkalies. 
(Milbauer,  Z.  anorg.  1904,  42.  450.) 

Uranyl  sulphide,  UO2S. 

SI.  sol.  in  pure  H2O.  Sol.  in  dil.,  insol.  in 
absolute  alcohol.  Sol.  in  cone.  HCl+Aq, 
also  in  dil.  acids.  Decomp.  by  caustic  al- 
kalies +Aq. .  Partly  sol.  in  (NH4)2S+Aq. 


Afetavanadic  acid,  HVO3. 

Insol.  in  H2O;  sol.  in  acids  and  alkalies. 

Insol.  in  liquid  NH3.     (Gore,  Am.  Ch.  J. 
1898,  20.  830.) 


See  Vanadium  pentoxide. 

Pyrovanadic  acid,  H4V2O7. 

Insol.  in  H2O.     Sol.  in  acids  and  alkalies. 

Vanadates. 

The  alkali,  Ba,  and  Pb  metavanadates  are 
si.  sol.  in  H2O,  the  others  are  more  easily  sol. 
Insol.  in  alcohol. 

Aluminum  we.'avanadate. 

Very  si.  sol.  in  H2O.     (Berzelius.) 

Aluminum  cfo'vanadate. 

Very  si.  sol.  in  H2O.     (Berzelius.) 

Ammonium  rae/avanadate,  (NH4)V03. 

(a)  Very  slowly  and  sparingly  sol.  in  cold 
H2O.  Easily  sol.  in  hot  H20.  (Berzelius.) 

Easily  sol.  in  H2O  at  about  70°.  Very  si. 
sol.  at  above  and  below  that  temperature. 
(Guyard,  Bull.  Soc.  (2)  25.  355.) 

10  g.  dissolve  in  1  litre  cold,  and  63  g.  in  1 
litre  hot  H2O  with  partial  decomp.  (Ditte,  C. 
R.  102.  918.) 

Solubility  in  H2O  at  t°. 


t° 

Solubility,  mol.  per 

litre 

18 

0.03715 

25 

0.05189 

35 

0.08980 

45 

0.13406 

55 

0.17041 

70 

0.25994 

(Meyer,  Z.  Elektrochem,  1909,  16.  266.) 
Solubility  in  NH4OH+Aq  at  t°. 


NH4OH+Aq 

t° 

Solubility, 
mol.  per  litre 

0.0677-N 
0.2452-N 
0.5872-N 

18 

0.04763 
0.06798 
0.1029 

0.0677-N 
0.2452-N 

0.5872-N 

25 

0.06026 
0.07303 
0.1080 

(Meyer,  Z.  Elektrochem,  1909,  15.  268.) 

Extremely  si.  sol.  in  sat.  NH4Cl+Aq.    (v. 
Hauer.) 

Insol.  in  sat.  NH4Cl+Aq. 


1104 


VANADATE,  AMMONIUM 


Solubility  in  salts  +Aq  at  t°. 

HVO3,  3NH3O,  2NH3  =  VO6N5H16.      Rap- 
idly    decomp.     by     H2O.      (Hofmann     and 
Kohlschutter.) 

Ammonium   potassium   vanadate,    K2V4On, 

(NH4)4V6017+9H20. 
Sol.  in  H2O.    (Ditte,  C.  R.  104.  1844.) 

Ammonium    sodium    vanadate,     Na2V4On, 
(NH4)4Ve017  +  15H20. 
Sol.  in  H2O.    (Ditte,  C.  R.  104.  1841.) 

Ammonium  uranyl  vanadate,  (NH4)2O,  2UO3, 
V205+H20. 
Insol.     in     H2O,     NH4OH+Aq,     or    dil. 
HO2H3O2+Aq.    (Carnot,  C.  R.  104.  1850.) 

Barium  raetavanadate,  Ba(VO3)2+H2O. 
Somewhat    sol.    in    H2O    before    ignition 
Sol.  in  cone.  H2SO4.     (Berzelius.) 

Salt  solution 

t° 

Solubility, 
mol.  per  litre 

0.05-NNH4Cl+Aq 

18 
25 
35 
45 
55 

0.01419 
0.02246 
0.04445 
0.07575 
0.09544 

0.1-NNH4Cl+Aq 

18 
25 
85 
45 
55 

0.00356 
0.00995 
0.02347 
0.04507 
0.06314 

0.05-NNH4NO3+Aq 

18 
25 

0.01433 
0.02364 

0.1-NNH4N03+Aq 

18 
25 

0.00497 
0.01050 

(Meyer,  Z.  Elektrochem,  1909,  16.  267.) 

Insol.  in  alcohol,    (v.  Hauer.) 
(6)  Sol.  in  cold  H2O,  from  which  it  is  pptd. 
by  alcohol.    (Berzelius.) 

Ammonium  ^vanadate,  (NH4)2V4On+4H20. 

Sol.  in  H2O,  from  which  it  is  precipitated 
by  sat.  NH4Cl+Aq  or  alcohol,  (v.  Hauer, 
W.  A.  B.  21.  337.) 

Correct  formula  is  "(NH4)3V7G,o+2H2O, 
accorcling  to  Rammelsberg  (B.  A.  B.  1883.  3.) 

+3H2O.  Very  sol.  in  H2O.  (Ditte,  C.  R. 
102.  918.) 

Ammonium  rfn'vanadate,  (NH4)2V6Oi6. 

Anhydrous.  Nearly  insol.  in  hot  or  cold 
H2O.  (Norblad,B.  8.  126.) 

1.5  g.  dissolve  in  1  litre  of  boiling  H2O 
(Ditte,  C.  R.  102.  918.) 

+5H2O.    Very  si.  sol.  in  H2O.    (Ditte.) 

+6H2O  (?).  Very  sol.  in  H20.  (v.  Hauer, 
W.  A.  B.  39.  455.) 

Could  not  be  obtained.  (Norblad:  also 
Rammelsberg,  B.  A.  B.  1883.  3.) 

Ammonium  vanadate,  (NH4)3V7Oi0+2H2O. 

Correct  formula  of  v.  Hauer's  ^vanadate, 
according  to  Rammelsberg  (B.  A.  B,  1883.  3) 

SI.  sol.  in  H2O. 

Ammonium    sesgiuvanadate,    (NH4)4V6On+ 

4  or  6H2O. 
Very  sol.  in  H2O.    (Ditte,  C.  R.  102.  918.) 

Ammonium    penta vanadate,   (NH4)4Vi0O27  + 
10H2O. 

Sol.  in  H2O.    (Rammelsberg,  B.  A.  B.  1883. 

3.) 

Ammonium  hydroxylamine  vanadate. 

V06N3H10. 

Rapidly  decomp.  by  H2O.  (Hofmann  and 
Kohlschutter,  Z.  anorg.  1898,  16.  472.) 


Barium  pyro vanadate,  Ba2V2O7. 
Somewhat  sol.  in  H2O.     (Roscoe.) 

Barium  vanadate,  Ba2V6Oi7+14H2O. 

(Ditte,  C.  R.  104.  1705.) 

Ba3VioO28  +  19H2O.  1  pt.  is  sol.  in  5200 
pts.  H2O  at  20-25°.  Much  more  sol.  in  hot, 
but  decomp.  by  boiling  H2O.  (v.  Hauer,  W. 
A.  B.  21.  344.) 

Sol.  in  about  5000  pts.  H2O.  (Manasse,  C. 
C.  1886.  773.) 

Ba4VioO29+2H2O.     (Norblad.) 

Bismuth  vanadate,  Bi,2(VO4)2. 

Min.  Pucherite.  Sol.  in  HCl+Aq  with 
evolution  of  Cl. 

Cadmium  vanadate,  Cd(VO3)2. 

(Ditte,  C.  R.  102.  918.) 

CdV6O16+24H2O.  SI.  sol.  in  H2O.  (Ditte, 
C.  R.  104.  1705.) 

Cadmium  potassium  vanadate,  CdK2V6Oi7+ 

+9H2O. 

(Radau,  A.  251.  148.) 

Cd3yioO28,  K6Vi0O28+27H2O.  1000  pts. 
H2O  dissolve  5.4  pts.  at  18°.  (Radau.) 

Cadmium    vanadate    bromide,    3Cd3(VO4)2, 
CdBr2. 

Very  sol.  in  dil.  acids,  (de  Schulten,  Bull. 
Soc.  1900,  (3)  23.  160.) 

Cadmium    vanadate    chloride,    3Cd3(VO4)2, 
CdCl2. 

Very  sol.  in  dil.  acids,  (de  Schulten,  Bull. 
Soc.  1900,  (3)  23.  159.) 

Caesium  raetavanadate,  CsVO3. 
(Chabrie",  A.  ch.  1902,  (7)  26.  228.) 


VANADATE,  LEAD  ZINC 


1105 


Calcium  wetavanadate,  Ca(VO3)2+4H2O. 

Much  more  sol.  than  Sr(VO3)2,  and  solu 
tion  is  not  precipitated  by  alcohol.  (Ber 
zelius.) 

+3H2O.  Sol.  in  H2O2;  insol.  in  alcohol 
(Scheuer,  Z.  anorg.  1898,  16.  304.) 

Calcium  p^/rovanadate,  Ca2V2O7+5H2O. 

Precipitate. 

+2H2O.  Very  sol.  in  dil.  acids.  (Ditte 
C.  R.  104.  1705.) 

+2^H2O.    (Roscoe.) 

Calcium  eftvanadate,  CaV4On+9H2O. 
Easily  sol.  in  H2O.    (v.  Hauer.) 
When  fused  is  nearly  insol.  in  H2O.     (v. 

Hauer.) 

+6H2O.    (Manasse,  A.  240.  23.) 

Calcium  frivanadate,  CaV6Oi7  +  12H2O. 
Very  sol.  in  H2O.    (Ditte,  C.  R.  104.  1705.) 

Calcium  vanadate,  Ca3V8O23+15H2O. 
Sol.  in  H2O.     (Manasse,  A.  204.  23.) 
Ca3V14O38+7H2O    (?).      SI.    sol.    in    H2O. 
Probably  a  mixture.     (Manasse,  A.  240.  23.) 
Ca3Vi*8O43+26H2O.     Sol.  in  H2O.     (Man- 
asse, A.  240.  23.) 

Calcium  copper  vanadate,  (Ca,  Cu)4V2O9+ 

H2O. 
Min.  Volborthite.    Sol.  in  HNO3+Aq. 

Calcium  potassium  vanadate.  CaK8V20O65  + 

22H20. 
Sol.  in  H2O.    (Manasse,  A.  240.  23.) 

Calcium  vanadate  chloride,  Ca3(VO4)2,  CaCl2. 
(Hautefeuille,  C.  R.  77.  896.) 

Chromium  vanadate,  CrVO4. 

Absolutely  insol.  in  H2O  containing 
NH4C2H3O;  and  HC2H3O2.  (Carnot,  C.  R. 
104.  1850.) 

Cobaltous  raetavanadate,  Co(VO3)2+3H2O. 

Easily  sol.  in  H2O.  (Ditte,  C.  R.  104. 
1705.) 

Cobaltous  potassium  vanadate,  CoKV6Oi4  + 

+8H2O. 

1000  pts.  H2O  dissolve  4.8  pts.  of  this  salt. 
\    (Radau,  A.  251.  140.) 

Co3K2Vi4O39+21H2O.    (Radau.) 

Cupric  wetavanadate. 
Sol.  in  H2O.    (Berzelius.) 

Cupric  p?/r0vanadate,  Cu2V2O7+3H2O. 
Sol.  in  hot  H2O.    (Ditte,  C.  R.  104.  1705.) 
Could  not  be  obtained.     (Radau,  A.  251. 

150.) 


Cupric  lead  vanadate,  5(Cu.  Pb)O.  V2O6+ 
2H2O. 

Min.  Mottramite. 

3CuO,  V205,  3(3PbO,  V205),  6CuO2H2  + 
12H2O.  Min.  Psittacinnite. 

Cupric    potassium    vanadate,    CuKV9O24+ 

171*20. 

Moderately  sol.  in  warm  H2O.  100  pts. 
H2O  dissolve  11.1  pts.  at  18°.  (Radau,  A. 
251.  151.) 

Didymium  vanadate,  Di2(VO4)2. 

Precipitate.    (Cleve.) 

Di2Vi0O30  +28H2O.  Precipitate.  (Cleve, 
Bull.  Soc.  (2)  43.  365.) 

Glucinum  metovanadate  (?). 

Difficultly  sol.  in  H2O.    (Berzelius.) 

Glucinum  cfo'vanadate  (?). 

Difficultly  sol.  in  H2O.    (Berzelius.) 

Indium  metovanadate,  In(VO3)3+2H2O. 
Ppt.     (Renz,.  Dissert.  1902.) 

Iron  (ferrous)  wetavanadate. 

Ppt.  Sol.  in  HCl+Aq.    (Berzelius.) 

Iron  (ferric)  wetovanadate. 

Somewhat  sol.  in  H2O.    (Berzelius.) 

Lead  wefovanadate,  Pb(VO3)2. 

SI.  sol.  in  H2O.  Easily  sol.  in  warm  dil. 
HNO3+Aq.  Not  completely  decomp.  by 
H2SO4  or  by  boiling  with  K2CO3+Aq/'  (Ber- 
zelius.) 

Min.  Dechenite.  Easily  sol.  in  dil.  HNO3+ 
Aq,  and  decomp.  by  HCl+Aq. 

Lead  p?/rovanadate,  basic,  2Pb2V2O7,  PbO. 

Insol.  in  boiling  H2O  or  HC2H3O2.  De- 
comp. by  HN03+Aq  with  separation  of  V2O5, 
which  dissolves  on  warming.  (Roscoe.) 

Lead  p?/rovanadate,  Pb2V2O7. 

Sol.  in  warm  dil.  HNO3+Aq.  (Ditte,  C.  R. 
104.  1705.) 

Min.  Descloizite.    Sol.  in  cold  dil.  HNO3+ 


Lead  ^vanadate,  PbV4On. 
(Ditte,  C.  R.  104.  1705.) 

Lead  or^ovanadate,  Pb3(VO4)2. 

Insol.  in  H2O.     (Roscoe,,  A.  suppl.  8.  109.) 

Lead  zinc  ortho  vanadate,  4Pb3(VO4)2, 

3Zn3(V04)2. 

Min.  Eusynchite.     Easily  sol.  in  HNO3+ 
Aq. 


1106 


VANADATE,  LEAD  ZINC 


Lead  zinc  vanadate,  (Pb,  Zn)4V2O9+H2O. 

Min.  Descloizite.  Sol.  in  excess  of  HNO3+ 
Aq. 

Lead  vanadate  chloride,  SFb.fVO,),,  PbCl2. 

Min.  Vanadinite.  Easily  sol.  in  HNO3+ 
Aq. 

Lithium  vanadate,  basic,  Li6V2O8+6H2O. 
Sol.  in  H2O.     (Ditte,  C.  R.  104.   1168.) 
Li8V2Os+H2O,  and  14H2O.     Sol.  in  H2O. 

(Ditte.) 

Lithium  metovanadate,  LiV08. 
Easily  sol.  in  H2O.    (Berzelius.) 
+2H2O.    Quite  easily  sol.  in  H2O.    (Ram- 

melsberg,  B.  A.  B.  1883.  3.) 

Lithium  divanadate,  Li2V4On+9H2O. 

Very  sol.  in  H2O.    (Norblad.) 

Correct  formula  is  Li3V5Oi4+12H2O. 
(Rammelsberg.) 

+8,  or  12H2O.     (Ditte,  C.  R.  104.  1168.) 

Lithium  or^ovanadate,  Li3VO4. 

Insol.  in  H2O.     (Rammelsberg,  B.  A.  B. 

-1.3.) 

Lithium  p*/rovanadate,  Li4V2O7-HH2O. 

Very  sol.  in  H2O.  (Rammelsberg,  B.  16. 
1676.) 

+3H2O.    (Ditte,  C.  P.  104.  1168.) 

Lithium  vanadate,  Li3V6O14+7H2O. 

Difficultly  sol.  in  H2O.    (Rammelsberg.) 

+  12H2O.  Very  efflorescent.  Correct  for- 
mula for  v.  Hauer's  cfo'vanadate.  (Rammels- 
berg.) 

Li4V6O17  +  16H2O.  Sol.  in  H2O.  (Ditte, 
C.  R.  104.  1168.) 

+  15H2O.    (Rammelsberg.) 

+  11H20.    (R.) 

+3H2O.    (R.) 

Li6V4Oi3  +  15H2O.  Not  very  easily  sol.  in 
H2O.  (Rammelsberg.) 

Li6V8O23  +  12H20 .  Moderately  sol.  in  H2O. 
(Rammelsberg . ) 

Lii0Vi2O35+30H2O.  Efflorescent.  Very 
sol.  in  H2O.  (Rammelsberg.) 

Magnesium  metovanadate,  Mg(VO3)2. 
Very  easily  sol.  in  H2O.    (Berzelius.) 
+6H2O.    Very  sol.  in  H2O.    (Ditte,  C.  R. 

104.  1705.) 


lesium  divanadate,  MgV4Ou+8H2O. 

Difficultly  sol.  in  H2O,  but  much  more  sol. 
than  barium  di vanadate.    (v.  Hauer.) 
+9H2O.    (Ditte,  C.  R.  104.  1705.) 

Magnesium  fnvanadate,  Mg2V6Oi7+4^H2O. 

Very  si.  sol.  in  H2O.     (Manasse,  A.  240. 

23.) 


Magnesium  vanadate,  Mg3Vi0O28+28H2O. 

Sol.  in  H2O.     (Suguira  and  Baker,  Chem. 
Soc.  35.  715.) 


M 


ous       raetavanadate,      Mn(VO3)2  + 


Very  si.  sol.  in  cold,  somewhat  more  sol.  in 
hot  H2O.  Easily  sol.  in  dil.  acids.  (Radau,  A. 
251.  125.) 

SI.  sol.  in  H2O2;  insol.  in  alcohol.  (Scheuer, 
Z.  anorg.  1898,  16.  304.) 

Manganous  pyrovanadate,  Mn2V2O7. 

SI.  sol.  in  hqt  dil.  HNO3+Aq.  (Ditte,  C.  R. 
96.  1048.) 

Manganous  potassium  vanadate,  MnKV6Oi4 

+8H2O. 
100  pts.  H2O  dissolve  1.7  pts.  salt  at  18°. 

Easily  sol.  in  acids.  (Radau,  A.  251.  129.) 
3Mn3V8O23,  K6V8O23+54H2O.  (Radau.) 
7Mn(VO3)2,  2KVO3+25H2O.  (Radau.) 
HMn(VO3)2,  2KVO3+48H2O.  (Radau.) 

Mercuric  vanadate. 

SI.  sol.  in  H2O. 

Nickel  vanadate,  Ni(VO8)2. 
Sol.  in  H2O.     (Ditte,  C.  R.  104.   1705.) 

Nickel  or^ovanadate,  Ni3(VO4)2. 

Insol.  in  H2O;  sol.  in  HN03+Aq.  (Ditte, 
C.  R.  96.  1049.) 


Nickel  (fcvanadate,  NiV4On+3H2O. 
Sol.  in  H2O.    (Ditte,  C.  R.  104.  1705.) 


Nickel  potassium  vanadate,   5Ni(V03)2, 
2KV03+25H2O. 

Ni3K2Vi0O29+17H2O.  Very  si.  sol.  in  hot 
H2O. 

NiKV5O4+8H2O. 

2Ni4V14O39,  K8Vi4O39+69H2O.  1000  pts. 
H2O  dissolve  1.7  pts.  of  salt  at  17.5°.  (Radau, 
A.  251.  137.) 

Potassium  vanadate,  basic,  K8V2O9+20H2O. 
Sol.  in  H2O.     (Ditte,  C.  R.  104.  902.) 


Potassium  metovanadate,  KV03. 

Anhydrous.  Slowly  sol.  in  cold,  more 
easily  in  hot  H2O.  Insol.  in  alcohol.  (Ber- 
zelius.) 

Completely  sol.  in  a  little  cold  H2O.  (Nor- 
blad.) 

+H2O.      Sol.    in    H2O.      (Rammelsberg.) 

+  1^H2O.     (Ditte.) 

+  1^H2O.     (Ditte.) 

+2H2O.     (Ditte.) 

+3H2O.    (Ditte,  C.  R.  104.  902.) 

+7H2O.     (Rammelsberg.) 


VANADATE,  SODIUM 


1107 


Potassium  (ftvanadate,  K2V4Oii+4H2O. 
Sol.  in  cold  or  lukewarm  H2O.    Decomp.  by 

hot  H2O.    (Rammelsberg.) 
+3H2O.     (Berzelius.) 
+3>iH2O.    Sol.  in  warm  H2O.    (Norblad.) 
+8  or  10H2O.     (Ditte,  C.  R.  104.  902.) 
+6H2O.    (Ephraim,  Z.  anorg.  1903,  35.  76.) 

Potassium  Znvanadate,  K2V6Oi6. 

Anhydrous.  Nearly  insol.  in  H2O.  (Nor- 
blad.) 

+6H2O.  Insol.  in  cold  or  hot  H2O.  (Nor- 
blad.) 

+  1,  and  5H2O.     (Ditte,  C.  R.  104.  902.) 

Potassium    or^ovanadate.   K3VO4+4^    or 
6H20.  § 

Deliquescent.  Sol.  in  H2O.  (Ditte,  C.  R. 
104.  902.) 

Decomp.  by  H2O  into  K4V2O7  and  KOH. 
(Rammelsberg,  B.  A.  B.  1883.  3.) 

Potassium  pyrovanadate,  K4V2O7+3H20. 

Deliquescent  Easily  sol.  in  H2O.  Insol. 
in  alcohol.  (Norblad.) 

+4H2O.    (Ditte,  C.  R.  104.  902.) 

Potassium  vanadate,  K3V5O14-f-5H2O. 

100  pts.  H2O  dissolve  19.2  pts.  at  17.5°. 
(Radau,  A.  251.  120.) 

-f-4^H2O.     (Radau.) 

K4V6O]7+2H2O.  Slowly  sol.  in  H2O. 
(Rammelsberg.) 

+6H2O.    (Ditte,  C.  R.  104.  902.) 

+7H2O.    (Friedheim.  B.  23.  1526.) 

K4VioO27  +  12H2O.  Very  sol.  in  H2O. 
(Manasse,  A.  240.  42.) 

K10V8O25+7H2O.    Sol.  inH2O.    (Rammels- 

K2V8O21+1^H2O.  Very  si.  sol.  in  H2O. 
(Ephraim,  Z.  anorg.  1903,  35.  75.) 

K4Vi8O47.  (Ephraim,  Z.  anorg.  1903, 
35.  78.) 

Potassium  sodium  vanadate,  2(2K2O,3V205), 

3(2Na2O,  3V2O5)+30H2O. 
(Friedheim,  Z.  anorg.  1894,  5.  442.) 
2K2O,    3V2O6,   4(2Na2O,    3V2O5)+35H2O. 

Efflorescent.      (Friedheim,    Z.    anorg.    1894, 

5.  441.) 

Potassium  strontium  vanadate,  K2Sr3Vi4O39+ 

20H2O. 

Sol.  in  H2O.    (Manasse,  A.  240.  23.) 
K2Sr3Vi4O39+30H2O.     As  above.     (Man- 
asse.) 

K4Sr2Vi4O39+18H2O.  As  above.  (Man- 
asse.) 

Potassium  zinc  vanadate,  KZnV6Oi4+8H2O. 

1000  pts.  H2O  dissolve  4.1  pts  of  the  salt. 
(Radau,  A.  251.  145.) 
2K8V14O39,  3Zn4V14O39+90H2O.     (Radau.) 


Potassium  vanadate  cyanide,  K4V2O7,  4KCN 
+14H2O. 

Easily  decomp. 

Insol.  in  alcohol.  (Petersen.  Z.  anorg. 
1904,  38.  343.) 

Samarium  vanadate,  Sm2O3,  5V2O6+28H2O. 

(Cleve.) 

+24H2O.     (Cleve.) 

Samarium  or^ovanadate. 
Precipitate. 

Silver  raetavanadate,  AgVO3. 

Sol.  in  HNO3  or  dil.  NH4OH+Aq.  (Ber- 
zelius.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  829.) 

Silver  or^ovanadate,  Ag3VO4. 

Ppt.  Easily  sol.  in  HNO3  or  NH4OH+Aq. 
(Roscoe,  Proc.  Roy.  Soc.  18.  316.) 

Silver  pyrovanadate,  Ag4V2O7. 

Ppt.    (Roscoe.) 

Sol.  in  NH4OH+Aq.  (Ditte,  C.  R.  104. 
1705.) 

Silver  vanadate,  Ag6V4Oi3. 

Sol.  in  21,414  pts.  H2O  at  14°,  and  13,617 
pts.  at  100°.  (Carnelley,  A.  166.  155.) 

Silver  vanadate  ammonia,  6AgVO3,  4NH3-f- 

8H20. 
(Ditte,  C.  R.  104.  1705.) 

Sodium   vanadate,    basic,    Na8V2O9+26    or 

30H2O. 
Very  sol.  in  H2O.    (Ditte.) 

Sodium  raetavanadate,  NaVO3. 

Anhydrous.  Slowly  sol.  in  cold,  very  easily 
in  hot  H2O.  (Norblad.) 

100  g.  H2O  dissolve  at: 
25°         40°         60°         75° 

21.10     26.23      32.97      38.83  g.  NaVO8. 
(McAdam  and  Pierle,  J.  Am.  Chem.  Soc. 
1912,  34.  606.) 

+2H2O.    Easily  sol.  in  H2O. 

100  g.  H2O  dissolve  at: 
25°          40°          60° 
15.23       29.93       68.36  g.  NaV03. 

At  75°  a  value  was  obtained  which  showed 
that  the  solid  phase  had  changed  into  the 
less  sol  modification.  (McAdam  and  Pierle, 
J.  Am.  Chem.  Soc.  1912,  34.  607.) 

+  ^H2O.    (Ditte,  C.  R.  104.  1061.) 

+3,  4,  and  5H2O.    (Ditte.) 

Sodium  efo'vanadate,  Na2V4On. 

Anhydrous.  SI.  sol.  even  in  warm  H2O, 
but  easily  sol.  on  addition  of  acids. 


1108 


VAN  ABATE,  SODIUM 


+9H2O.     Easily  sol.  in  cold  H2O.     Insol. 

in  alcohol.     (Norblad.) 

+5H2O.     (Ditte,  C.  R.  104.  1061.) 

Not  obtained  by  Rammelsberg  (B.  A.  B. 

1883.  3.) 

Sodium  Jrivanadate,  Na2V6Oi6+9H2O. 
Insol.  in  cold  or  hot  H2O.     (Norblad.) 
Composition  is  Na6V16O43+24H2O.    (Ram- 
melsberg.) 

+3H2O.     (Ditte,  C.  R.  104.  1061.) 

Sodium  ori/wvanadate,  Na3VO4+16H2O. 

Easily    sol.    in    H2O,    but    decomp.    into 
Na4V2O7  and  KOH.     Precipitated  by  an  ex- 
cess of  alcohol.    (Roscoe,  A.  suppl.  8.  102.) 
+7H2O.    (Hall,  Chem.  Soc.  61.  96.) 
+  10.,  and  12H2O.    Less  sol.  in  dil.  NaOH 
+Aq  than  in    H2O.     (Baker,  A.  229.  286.) 

Sodium  p?/rovanadate,  Na4V2O7-f-18H2O. 

Easily  sol.  in  H2O.  Insol.  in  alcohol. 
(Norblad.) 

Spl.  in  alcDhol.     (Ditte,  C.,  R.  104.  1061.) 

+8H2O.     (Ditte.) 

Sodium  sesgmvanadate,  Na4V6Oi7. 

Anhydrous.  Insol.  in  H2O  or  NH4OH+Aq. 
(Rammelsberg.) 

+  10H2O.     (Norblad.) 

+  16H2O.     Efflorescent.     (Rammelsberg.) 

+  18H2O.     (Ditte.) 

Sodium  pentavanadate,  Na4Vi0O27+3V2H2O. 
Scarcely  sol.  in  H2O.    (Rammelsberg.) 

Sodium  vanadate,  Na6V4Oi3-j-6H2O. 

Difficultly  sol.  in  cold  H2O.  (Carnelley, 
A.  166.  155.) 

+2H2O.     (Carnelley.) 

Na6Vi6O43+24H2O.  Correct  formula  for 
Norblad' s  ^nvanadate.  (Rammelsberg.) 

Na2O,  4VaO«+7^H2O:  (Baragiola,  Dis- 
sert. 1902.) 

+8MH2O.    (Baragiola.) 

3Na2O;  5V2O6+22H2O.  (Prandtl  and 
Lustig,  Z.  anorg.  1907,  53.  405.) 

4Na2O,  7V2O5+33H2O.  (Friedheim,  Z. 
anorg.  1894,  6.  443.) 

5Na2O,  8V2O6+39H2O.  Sol.  in  H2O 
(Friedheim,  Z.  anorg.  1894,  5.  441.) 

Sodium  vanadate  fluoride,  2Na3VO4,  NaF+ 
19H20. 

Sol.  in  H20.  (Rammelsberg,  W.  Ann.  20. 
928.) 

Stontium  metavanadate,  Sr(VO3)2+4H2O. 
Difficultly  sol.  in  cold  H2O.     (Norblad.) 

Strontium  divanadate,  SrV4On+9H2O. 

SI.  sol.  in  H2O,  but  much  more  sol.  than 
barium  di'vanadate.  (v.  Hauer.) 


Sol.  in  H2O2+Aq  free  from  H2SO4. 
Insol.  in  alcohol.  (Scheuer,  Z.  anorg.  1898, 
16.  303.) 

Strontium  £nvanadate,  SrV6Oi6+14H2O. 

Sol.  in  H2O,  but  decomposes  slowly  on 
boiling.  Easily  sol.  in  hot  H2O  acidified 
with  HC2H3O2,  and  crystallizes  therefrom 
without  decomp.  (v.  Hauer,  J.  pr.  76.  156.) 

Strontium  fctfravanadate,  SrV8O2i  +  llH20. 

Sol.  in  hot  H2O  with  partial  decomposition. 
(Manasse,  A.  240.  34.) 

Strontium  vanadate,  Sr3V8O23+14H2O. 
Sol.  in  H2O.    (Manasse,  A.  240.  23.) 
Sr4V14O39+30H2O.      Sol.   in   H2O.      (Nor- 
blad.) 

Thallous  metovanadate,  T1VO3. 

Sol.  in  11,534  pts.  H2O  at  11°,  and  4756 
pts.  at  100°.  (Carnelley.) 

Thallous  or^ovanadate,  T13VO4. 

SI.  sol.  in  H2O.  Sol.  in  999  pts.  H2O  at  15°, 
and  574  p  s.  at  100°.  (Carnelley,  Chem. 
Soc.  (2)  11.  323.) 

Thallous  p2/rovanadate,  T14V2O7. 

Sol.  in  4996  pts.  H2O  at  14°,  and  3840  pts. 
H2O  at  100°.  (Carnelley.) 

Thallous  vanadate,  Tli2V8O26. 

Sol.  in  3406  pts.  H2O  at  14°,  and  533  pts. 
at  100°.  (Carnelley.) 

Tl12V10O3i.  Sol.  in  9372  pts.  H2O  at  11°, 
and  3366  pts.  at  100°.  (Carnelley.) 

Tl12Vi4O4i.    Ppt.     (Carnelley) 

Thorium  vanadate,  Th3O12(VO)4,  16V2O6-f 
24H2O  (?). 

Sol.  in  H2O.     (Cleve.) 

ThO2,V2O5+6H2O.  Sol.  in  acids.  (Volck, 
Z.  anorg.  1894  6.  167. 

Uranyl  vanadate,  2UO3,  V2O6,   (UO2)2V2O7. 
Insol.  in  H2O.    "(Garnet,  C.  R.  104.  1850.) 

Vanadium  vanadate,  2VO2,  V2O6=V4O9. 

Insol.  in  H2O.    Sol.  in  dil.  H2SO4  or  HNO3 

Aq.     (Rammeslberg.) 

Slowly  oxidised  by  HNO3+Aq.  Slowly 
sol.  in  NH4OH+Aq.  Reasily  sol.  in  HCl+Aq 
(Ditte,  C.  R.  101.  1487.) 

+22/3H2O.     (Brierley.) 

2VO2,  2V2O6+8H2O.  Insol.  in  H2O. 
(Brierley,  Chem.  Soc.  49.  31.) 

Ytterbium  vanadate,  3Yb2O3,  5V2O6+3H2O. 

Yb2O3,  15VoO6.  Ppt.  (Cleve,  Z.  anorg. 
1902,  32.  150.) 

Yttrium  vanadate. 

Precipitate.     (Berzelius.) 


VANADIOMOLYBDATE,  AMMONIUM 


1109 


Zinc  vanadate,  Zn(VO3)2-f  2H2O. 
Sol.  in  H2O.    (Ditte,  C.  R.  104.  1705.) 

Zinc  pyrovaaadate,  Zn2V2O7. 

Appreciably  sol.  in  H2O.  (Ditte,  C.  R. 
96.  1048.,) 

Pervanadic  acid. 
See  Pervanadic  acid. 

Vanadicotungstic  acid. 

Ammonium  vanadicotungstate, 

3(NH4)2O,  V2O3,  8WO3+10H2O. 

Very  sol.  in  H2O. 

Insol.  in  organic  solvents.  (E.  F.  Smith, 
J.  Am.  Chem.  Soc.  1903,  26.  1227.) 

Vanadicovanadic  acid. 

Ammonium    vanadicovanadate,    (NH4)2O, 
2VO2,  4V2O6+8H2O. 

SI.  sol.  in  cold  and  warm  H2O.  (Gibbs, 
Am.  Ch.  J.  7.  209.) 

(NH4)2O,  2V2O4,  2V2O6+14H2O.  Sol  in 
H2O.  (Brierley,  Chem.  Soc.  49.  30.) 

3(NH4)2O,  2V2O4,  4V2O8+6H2O.  Insol. 
in  H2O.  (Brierley.) 

Potassium ,  2K2O,  2V2O4,  V2O5+6H2O. 

Sol.  in  hot  H3O.  (Brierley,  Chem.  Soc. 
49.  30.) 

5K2O,  2V2O4,  4V2O5+H2O.  Insol.  in  H2O. 
.(Brierley.) 

K2O,  V2O4,  8V2O5.      Insol.  in  H2O. 

Sol.  in  cone.  H2SO4.  (Prandtl,  B.  1905, 
38.  660.) 

Sodium ,  2Na2O,  2V2O4,  V2O6+13H2O. 

Easily  sol.  in  H2O.  Insol.  in  cone,  solu- 
tions of  salts,  especially  acetate.  (Brierley, 
Chem.  Soc.  49.  30.) 

2Na2O,  V2O4,  5V2O6.  Insol.  in  H2O.  Sol. 
in  cone.  H2SO4.  Not  attacked  by  boiling 
with  cone.  HNOg.  Slowly  attacked  by  hot 
dil.  NH4OH-fAq.  (Prandtl,  B.  1905,  38. 
659.) 

Vanadioarsenic  acid. 
See  Arseniovanadic  acid. 

Vanadioiodic  acid. 

See  lodovanadic  acid. 

Vanadiomolybdic  acid,  8MoO3,  V2O6+ 
5H2O. 

Very  si.  sol, -in  H2O,  and  si.  sol.  in  boiling 
HNO3+Aq.  (Ditte,  C.  R.  102.  757.) 

Could  not  be  obtained.  (Friedheim,  B. 
24.  1173.) 

Ammonium  vanadiomolybdate, 

(NH4)2O,  V2O5,  2MoO3+4H2O. 
Nearly   insol.    in    H2O.      (Friedheim   and 
Castendyck,  B.  1900,.  33.  1615.) 


(NH4)20,  2V206,  2Mo03+8H20.  Nearly 
insol.  in  H2O.  (Friedheim  and  Castendyck.) 

2(NH4)2O,  V2O5,  3MoO3+6H2O.  (Euler- 
Chelpin,  Dissert,  1896.) 

(NH4)20,  V205,  3Mo03+17H20.  (Euler- 
Chelpin.) 

2(NH4)2O,  V2O5,  4MoO3+7H2O  and  + 
8H2O.  (Euler-Chelpin,) 

3(NH4)20,  2V205,  4Mo03+7H20.  (Milch, 
Dissert.  Berlin,  1887.) 

+9H2O.  Sol.  inH2O.  (Ditte,  C.  R.  102. 
1019.) 

+  11H2O.  Easily  sol.  in  H2O.  Correct 
composition  of  above  compounds  is  = 
(NH4)2O,  2V2O5+2[NH4)2O,  2MoO3]+llH2O. 
(Friedheim,  B.  24.  1173.) 

Moderately  sol.  in  H2O  and  can  be  re- 
cryst.  therefrom.  (Euler-Chelpin,  Dissert, 
1895.) 

2(NH4)2O,  3V2O5/.  4MoO3fllH2O.  Near- 
ly insol.  in  H2O.  (Friedheim  and  Casten- 
dyck, B.  1900,  33.  1615.) 

2(NH4)2O,  2V2O5,  5MoO3.  Nearly  insol. 
in  cold  H2O.  (Euler-Chelpin,  Dissert.  1896.) 

+8H2O.  Nearly  insol.  in  H2O.  (Fried- 
heim and  Castendyck,  B.  1900,  33.  1615.) 

3(NH4)2O,  2V2O5,  5MoO3+8>iH2O.  Very 
easily  sol.  in  H2O.  (Liebert,  Dissert.  1891.) 

4(NH4)2O,  12V2O5,  5MoO3+24HiO.  Prac- 
tically insol.  in  H2O.  (Friedheim  and  Casten- 
dyck, B.  1900,  33.  1615.) 

2(NH4)2O,  V2O6,  6MoO3+5H2O.  Sol. 
in  a  large  amount  of  H2O.  (Gibbs,  Am.  Ch. 
J.  6.  361.) 

+6H2O.    Rather  si.  sol.  in  H2O. 

Easily  sol.  in  acids.  (Liebert,  Dissert, 
1891.) 

Composition  is  double  the  above  formula, 

°r4(NH4)2O,  2V2O5,  12MoO3+12H2O. 
Rather  difficultly  sol.  in  H2O.  Composition 
is  (NH4)2O,  2V2O6+3[NH4)2O,  4MoO3]. 
(Friedheim.) 

3(NH4)2O,  V2O5,  6MoO3+7H2O.  (Isen- 
burg,  Dissert,  1901.) 

5(NH4)2O,  4V2O5,  6MoO3+12H2O  and 
+  14H2O.  (Euler-Chelpin,  Dissert,  1896.) 

5(NH4)2O,  3V2O6,  7MoO3+13H2O  and 
+  16H2O.  Sol.  in  H2O  and  can  be  recryst. 
therefrom.  (Toggenburg,  Dissert,  1902.) 

5(NH4)2O,     3V2O6,     8MoO3+14H2O. 
(Stamm,  Dissert,  1906.) 

5(NH4)2O,  2V2O5,  12MoO3flOH2O.  Quite 
easily  sol.  in  H2O.  Composition  is  (NH4)2O, 
2V2O5+4[(NH4)2O,  3MoO3]  +  10H2O. 

6(NH4)20,  3V205,  12Mo03+21H20.  Sol. 
in  H2O.  Composition  is  (NH4)2O,  3V2O5+ 
5(NH4)2O,  12MoO3.  (F.) 

8(NH4)2O,  4V2O6,  13MoO3+21H2O.  Sol. 
in  H2O.  (Isenburg,  Dissert,  1901.) 

8(NH4)2O,  V2O6,  18MoO6  +  15H2O.  De- 
comp.  by  hot  H2O.  (Gibbs.)  Could  not 
be  obtained.  (Friedheim.) 

10(NH4)2O,  3V2O6,  24MoO3+10H2O.  Sol. 
in  H2O.  (Milch.)  Could  not  be  obtained. 
(Friedheim.) 


1110 


VANADIOMOLYBDATE,  AMMONIUM  BARIUM 


Ammonium  barium  vanadiomolybdate, 
5(NH4)2O,  15BaO,  6V205,  36MoO3. 

(Milch.) 

(NH4)2O,   BaO,   V2O5,   MoO3+6H2O. 
(Euler-Chelpin,  Dissert,  1895.) 

3(NH4)2O,  BaO.  3V2O6,  5MoO3+9H2O. 
SI.  sol.  in  oold  and  hot  H2O.    (Euler-Chelpin.) 

Ammonium  potassium ,  (NH4)aO,  3K20, 

2V2O6,  4Mo03+5H2O. 
Decomp.  by  H2O.    (Euler-Chelpin,) 
(NH4)2O.    3K2O,    3V205,    5MoO3+9H2O. 

(Euler-Chelpin.) 
K(NH4)2O,     3KK2O,     3V2O6,     5Mo03+ 

16H2O.      Sol.    in    H2O.     (Jacoby,    Dissert. 

1900.) 

Ammonium  sodium  ,   (NH4)2O,  Na2O, 

2V2O6,  6Mo03+12H20. 
(Euler-Chelpin,  Dissert,  1896.) 

Barium ,  BaO,  V206,  MoO3+7H2O. 

(Euler-Chelpin.) 

Barium ,  3BaO,  2V2O6,  6Mo03. 

(Milch.) 

+8H2O.    (Euler-Chelpin.) 

5BaO,  4V2O5,  6MoO3+28H2O.  Sol.  in 
hot  H2O.  (Euler-Chelpin.) 

3BaO,  V2O5,  8MoO3+2BaO,  H2O,  V2O5, 
8MoO3+28H2O.  Sol.  in  hot  H2O.  (Gibbs, 
Am.  Ch.  J.  6.  361.) 

7BaO,  3V2O5,  18MoO3+16H2O  =  BaO, 
3V2O5+6(BaO,  3MoO3)  +  16H2O.  SI.  sol. 
in  H2O. 

+36H2O  and  +48H2O.  (Liebert,  Dis- 
sert. 1891.) 

Potassium ,  K2O,  V2O5,  3Mo03+15H2O. 

Nearly  insol.  in  cold  H20.  (Euler-Chelpin, 
Dissert,  1896.) 

3K2O,  2V2O5,  4MoO3+8H2O=K2O,  2V205 
-t-2(K2O,  2MoO3)+8H2O. 

Very  sol.  in  H2O.    (Friedheim.) 

+7H2O.  Easily  sol.  in  cold  H2O.  (Euler- 
Chelpin.) 

+9H2O;  Easily  sol.  in  cold  H2O.  (Euler- 
Chelpin.) 

2K2O,  2V2O6,  5MoO3+10H2O.  Nearly 
insol.  in  cold,  very  si.  sol.  in  hot  H2O.  (Euler- 
Chelpin.) 

3K  A  V2OS,  6MoO3+5H2O.  (Euler-Chel- 
pin.) 

2K2O,  V2O5,  6MoO3+6H2O.  Very  si.  sol, 
in  cold,  easily  sol.  in  hot  H2O.  (Liebert.) 

4K20,  2V2O8,  12MoO3+12H2O=K2O, 
2V2O5+3(K2O,  4Mo03)-f-12H2O.  SI.  sol, 
in  H2O.  (Friedheim.) 

5K20,  2V2O5.  12MoQ3  +  12H2O=K20, 
2V2O+4(K2O,  3MoO3)  +  12H2O.  Rather  si, 
sol.  in  H20.  (Friedheim.) 

SI.  sol.  in  cold,  easily  sol.  in  hot  H2O. 
(Liebert,  Dissert,  1891.) 

3K2O,  V2O6,  12MoO3  +  15H20.     (Liebert.) 


Potassium  sodium  vanadiomolybdate,  K2O, 

4Na2O,  2V2O6,  12Mo03  +  18H2O. 
(Euler-Chelpin.  Dissert  1895.) 

Sodium  •,  2Na2O,  V2O5,  6MoO3+16H2O. 

(Euler-Cheipin,  Dissert,  1895.) 

Vanadiophosphoric  acid. 
See  Phosphovanadic  acid. 

Vanadioselenious  acid,  3V2O6,  4SeO2-f- 
4H20. 

+6H2O.  Difficultly  sol.  in  H2O.  Can  b< 
cryst.  from  H2O. 

+  10H2O.  Difficultly  sol.  in  H20.  Can  b< 
cryst.  from  H2O.  (Prandtl,  B.  1905,  38 
1307.) 

Ammonium  vanadioselenite, 

4(NH4)2O,  6V2O6,  5SeO2+13H2O. 

SI.  sol.  in  H2O.    Decomp.  by  boiling  H2O 

3(NH4)2O.  3V2O5.  6SeO2+2H2O.  Ppt 
(Prandtl,  B.  1905,  38.  1309.) 

(NH4)3HV6O17,  12SeO2+2H2O.     Ppt. 

+4H2O.  Ppt.  (Prandtl,  Z.  anorg.  1911 
73.  231.) 

Ammonium  silver ^22/3(NH4)2O,  li/3Ag2O 

6V2O6,      5SeO2+12H2O,+16H2O      am 
+22H2O. 
(Prandtl,  Z.  anorg.  1907,  63.  402.) 

Lithium ,  4Li20,  6V2O5,  5SeO2+30H2O 

Very.  sol.  in  H2O.     (Prandtl.) 

Potassium    ,    4K2O,    6V2O5,    5SeO2-f 

13H20. 

3K2O,  3V2O5,  6SeO2.  (Prandtl,  B.  1905 
38.  1309.) 

Sodium ,  4Na2O,  6V2O5,  5SeO2+20H20 

Very.  sol.  in  H2O.  (Prandtl,  Z.  anore 
1907,  63.  403.) 

Vanadiosulphuric  acid,  V206,  3S03+3H20 
Deliquescent.    Sol.  in  H2O,  but  is  decomp 

by  boiling.     (Ditte,  C.  B,.  102.  757.) 
See  Sulphate,  vanadium. 

Vanadiosulpurous  acid. 

Ammonium  vanadiosulphite, 

3(V204,S02),  (NH4)20,  S02+4H20. 
(Gain,  C.  R.  1907,  144.  1158.) 

Caesium  ,  (V2O4,SO2),  3(Cs20,S02)  + 

8H2O. 

(Gain.) 

Lithium  ,  (V204,S02),  5(Li20,S02)  + 

8H2O. 

(Gain.)' 


VANADIOTUNGSTATE,  SODIUM 


1111 


Potassium      vanadiosulphite, 

SO2,(K2O)+5H2O. 
(Gain.) 


3S02,(V204), 


-,  (V204,S02),  2(Rb20,S02) 


Rubidium 
2H2O. 

(Gain.) 


Sodium    ,    5(V204,S02),    (Na20,SO2)  + 

2H2O. 

(Gain.) 

Thallium  ,    3(V2O4,SO2),    (T120,SO2)  + 

8H2O. 

(Gain.) 

Vanadiotungstic  acid,  6H20,  V2O6,  10WO8 
+16H2O. 

Very  si.  sol.  in  cold,  more  easily  in  hot  H2O. 
(Gibbs,  Am.  Ch.  J.  6.  361.) 

6H2O.  V2O5,  16WO3+30H2O.  Readily 
sol.  in  H2O.  (Gibbs.) 

17H2O.  4V2O5,  16WO3+24H2O.  SI.  sol. 
in  cold,  easily  in  hot  H2O.  (Rosenheim,  A. 
251.  228.) 

Aluminum  sodium  vanadiotungstate,  7A12O3, 
27Na20,  36V206,  144WO3+504H2O= 

3(A1203,  9Na20,  48W03),  4(A12O3,  9V2O5) 
+504H2O. 
Sol.  in  H2O.     (Rothenbach,  B.  23.  3055.) 


-,  (NH4)20,  3V205,  W03  + 


Ammonium 
6H2O. 

Sol.  in  H2O.  (Rammelsberg,  B.  1.  158.) 
2(NH4)2O,  V2O6,  4WO3+4H2O.  (Friedheim 
and  Lowy,  Z.  anorg.  1984.  6.  24.) 

4(NH4)2O.  2H20.  V2O5,  5WO3  +  11H2O. 
Sol.  in  H20.  (Gibbs.  Am.  Ch.  J.  6.  361.) 

2(NH4)2O.  V2O6,  5WO3+10H2O.  Sol.  in 
H20.  (Ditte,  C.  R.  102.  1019.) 

31(NH4)20,  14V205.  60W03+58H20  = 
5[5(NH4)»0,  12WO,],  2[3(NH4)20,  7V208)]. 
Sol  in  H2O.  (Rothenbach,  B.  23.  3051.) 

7(NH4)2O,  4V2O5,  14WO3  +  16H2O.  Sol. 
in  H2O.  (Rosenheim,  A.  261.  197.) 

8(NH4)2O,  4V2O5,  16WO3,  9H2O+4H2O. 
Efflorescent.  Very  sol.  in  H2O.  (Rosenheim, 
A.  251.  216.) 

Barium    ,    19BaO,     10V2O6,    36WO3  + 

94H20  =  3(5BaO,      12WO8),      2(2BaO, 
5V205)+94H20. 

SI  sol  in  H2O.    (Rothenbach,  B.  23.  3052.) 

8BaO,'     4V205,      16WO3,     9H2O+44H2O. 

Efflorescent.    Not  very  sol.  in  H2O.    (Rosen- 

hCCom^oStion2  is'  6BaO,  12WO3,  3V2O6  + 
39H2O.  (Friedheim.) 

6BaO  3V205,- 12WO3+34H2O.  Not  easily 
sol.  in  H2O.  (Friedheim  and  Lowy,  Z. 
anorg.  1894,  6.7 18.) 

4BaO,  4V2O6,   12WO3-f41H2O.     Less  sol. 


than  preceding  salt.    Decomp.  by  boiling  or 
by  mineral  acids.     (Rosenheim.) 

Composition  is  4BaO,  12WO3,  3V2O6  + 
30H2O.  (Friedheim.) 

Calcium     vanadiotungstate,     2CaO,     V2O6. 

2W08  +  12H20. 
(Friedheim  and  L6wy,  Z.  anorg.  1894,  6. 

Magnesium    sodium    ,    MgO,    6Na20, 

3V206,    12W08+42H20=5Na20, 
12W08+MgO,  Na20,  3V2O6+42H2O. 
Sol.  in  H2O.     (Rothenbach,  B.  23.  3054. 

Potassium  ,  4K2O,  3V206,  12WO8+ 

30H2O. 

Sol.  in  H2O. 

Composition  is  potassium  metatungstate 
vanadate,  3(K2O,  4WO3)+K2O,  3V2O6  + 
30H2O.  (Friedheim,  B.  23.  1515.) 

SKA  4V2O6, 16WO3, 9H2O  +24H2O.  Very 
efflorescent.  Easily  sol.  in  H2O,  (Rosen- 
heim, A.  251.  214.) 

Formula  is  6K2O,  12WO3,  3V2O5+24H2O, 
which  is  a  double  salt,  5K2O,  12WO3+K2O, 
3V2O5.  (Friedheim,  B.  23.  1505.) 

Potassium    sodium    ,    (5Na2O,    3V206, 

6WO3+22H2O),  4(5K2O,  3V206,  6WO8 
+22H2O)  or  Na2O,  4K2O,  3V2O6,  6WO, 
+22H20. 

(Friedheim  and  Lowy,  Z.  anorg.  1894,  6. 
22.) 

4(5Na2O,  3V2O5,  6WO3+24H2O),  3(5K20, 
3V2O6,  6W03+24H2O.)  (Friedheim  and 
Lowy.) 

5(5Na2O,  3V2O5,  6WO3+24H2O),  5K2O, 
3V2O5,  6WO3+24H2Q.  (Friedheim  and 
Lowy.) 

Silver  — ,  8Ag2O,  4V2O6,  16WO8,  9H2O. 

Somewhat  sol.  in  cold  H2O,  more  easily 
upon  addition  of  little  HNO3.  Decomp.  by 
warm  H2O.  (Rosenheim,  A.  251.  224.) 

3Ag?O,  2V2O5,  6WO3+3H2O.  Nearly 
insol.  in  cold  H2O.  Decomp.  by  addition  of 
HNO3  or  upon  warming.  (Rosenheim.) 

Sodium  — ,  5Na2O,  3V2O6,  6WO8+36H2O. 

Sol.  in  H2O. 

Composition  is  3(Na2O,  2WO3)+2(Na2O, 
3V2O5)+36H2O.  (Friedheim,  B.  23.  1527.) 

+38H2O.  Sol.  in  1.25  pts.  H2O  at  13.8°. 
(Friedheim  and  Lowy.) 

2Na2O,  2V2O6,  3WO3+2QH2O.  Very  sol, 
in  H2O. 

Composition  is  Na2O,  3WO3-j-Na2O,  2V2O6 
+20H2O,  double  salt  of  sodium  ^ntungstate 
and  divanadate.  (Friedheim,  B.  23.  1523.) 

4Na20,  3V205,  12WO3+38H2O=3(Na2O, 
4WO3)+Na2O,  3V2O6+38H8Q.  Sol.  in  H2O. 
(Rpjbhenbach,  B.  23.  3050.) 

aO,    4V206,    16W03,:    9K2O+48H2O. 


1112 


VANADIOTUNGSTATE,  STRONTIUM 


Efflorescent.  Easily  sol.  to  H2O.  (Rosen- 
heim,  A.  251.  210.) 

Formula  is  6Na2O,  12WO3,  3y2O6+42H20, 
and  is  a  double  salt  of  sodium  paratungstate, 
5Na2O,  12WO3,  and  sodium  ^nvanadate. 
Na2O,  3V2O6.  (Friedheim,  B.  23.  1505.) 

7Na20,  V205,  12W03+29H20.  Easily 
sol.  in  H2O.  (Friedheim  and  Lowy,  Z.  anorg. 
1894,  6.  15.) 

8Na2O,  V2O5,  14WO3+60H2O  and  +66H2O 
(Friedheim  and  Lowy.) 

Strontium  vanadiotungstate,  19SrO,  36WO3, 
10V2O6+122H2O  =  3(5SrO,         12WO3), 
2(2SrO,  5V206)+122H20. 
Sol.  in  H2O.     (Rothenbach,  B.  23.  3053.) 

Vanadious  acid. 
See  Hypovanadic  acid. 

Vanadiovanadicomolybdic  acid. 

Ammonium  vanadiovanadicomolybdate, 

11(NH4)A     4V205,     V02,     28Mo03  + 
48H2O. 
SI.  sol.  in  cold,  sol.  in  hot  H2O  without 

decomp.    (Gibbs,  Am.  Ch.  J.  5.  391.) 

Barium ,  14BaO,  2V2O5,  3VO2,  3QMoO3 

+48H20. 

Precipitate.  Very  si.  sol.  in  cold,  decomp. 
byhotH2O.  (Gibbs.) 

Vanadiovanadicotungstic  acid. 

Ammonium  vanadiovanadicotungstate, 

6(NH4)20,     2V206,     3V02,     12WO3  + 
12H2O. 
Sol.  in  H2O.     (Gibbs,  Am.  Ch.  J.  5.  S91.) 

Silver ,  6Ag20,  2V2O6,   3VO2,   12WO3+ 

8H20. 

Precipitate.  Very  si.  sol.  in  cold,  sol.  in 
much  warm  H2O.  (Gibbs.) 

Sodium ,  6Na20,  2V2O6,  3V02,  12WO3. 

Very  sol.  in  H2O.     (Gibbs.) 

Vanadium,  V. 

Insol.  in  H2O,  HC1,  dil.  H2SO4+Aq,  and 
cold  cone.  H2SO4.  Sol.  in  hot  cone.  H2SO4. 
Slowly  sol.  in  HF+Aq.  Easily  sol.  in  dil. 
or  cone.  HNO3+Aq.  Not  attacked  by  hot 
or  cold  NaOH  or  KOH+Aq.  (Roscoe,  A. 
suppl.  7.  85.) 

Does  not  alter  in  the  air;  not  acted  upon 
by  HC1  and  very  slowly  by  H2SO4.  (Moissan, 
C.  R.  1896,  122.  1299.) 

Vanadium  boride,  VB. 

Sol.  in  HF  and  HNO3.  Decomp.  by  fused 
alkalies.  (Wedekind,  B.  1913,  46.  1203.) 


Vanadium  ^bromide,  VBr3. 

Very  deliquescent;  quickly  decomposes. 
(Roscoe,  A.  suppl.  8.  99.) 

+6H2O.  Sol.  in  H20  with  decomp.  (Locke 
and  Edwards  Am.  Ch.  J.  1898,  20.  600.) 

Sol.  in  H2O,  alcohol  and  ether.  Insol.  in 
HBr.  (Piccini,  Z.  anorg.  1899,  19.  398.) 

Vanadium  carbide,  VC. 

Insol.  in  HC1  and  H2SO4. 

Sol.  in  HNO3  in  the  cold,  and  in  fused 
KNO3  and  KC1O3.  (Moissan,  C.  R.  1896, 
122.  1300.) 

Vanadium  ^chloride,  VC12. 

Very  deliquescent.  Sol.  in  H2O,  alcohol, 
and  ether.  (Roscoe,  A.  suppl.  7.  79.) 

Vanadium  bichloride,  VC13. 

Deliquescent.  Sol.  in  H2O,  absolute  alco- 
hol, and  ether. 

+6H2O.  Sol.  in  H2O;  si.  sol.  in  cone.  HC1+ 
Aq. 

Sol.  in  alcohol  and  ether.  (Piccini,  Z. 
anorg.  1899,  19.  395.) 

Vanadium  ^rachloride,  VC14. 

Sol.  with  decomp.  in  H2O,  alcohol,  and 
ether.  (Roscoe.) 

Sol.  in  H2Q  with  decomp. 

Sol.  in  fuming  HC1  with  decomp. 

Sol.  in  anhydrous  CHC13  or  glacial  acetic 
acid  apparently  without  chemical  change. 
(Koppel,  Z.  anorg.  1905,  46.  346.) 

Vanadium  cfo'fluoride,  VF2. 

Sol.  in  HF  with  evolution  of  H2  and  forma- 
tion of  VF3.  (Manchot,  A.  1907,  367.  135.) 

Vanadium  Znfluoride,  VF3. 

Nearly  insol.  in  H2O  and  organic  solvents. 
(Ruff,  B.  1911,  44.  2544.) 

+3H2O.  Efflorescent.  Easily  sol.  in  cold, 
extremely  sol.  in  hot  H2O  with  decomp. 
Can  be  recryst.  from  HF+Aq.  Insol.  in 
strong  alcohol.  (Petersen,  J.  pr.  (2)  40.  48.) 

Vanadium  teirafluoride,  VF4. 

Very  hydroscopic. 

Easily  sol.  in  H2O. 

Difficultly  sol.  in  SO2C12  and  SiCl4. 

Sol.  in  POC13  with  evolution  of  gas. 

Sol.  in  acetone  and  acetic  acid. 

Difficultly  sol.  in  alcohol  and  CHC13. 
(Ruff,  B.  1911,44.2545.) 

Vanadium  pe/Uafluoride,  VF5. 

Easily  sol.  in  H2O. 

Easily  sol.  in  alcohol,  CHC13,  acetone,  and 
ligroin.  Insol.  in  CS2.  Decomp.  toluene 
and  ether.  (Ruff,  B.  1911,  44.  2549.) 

Vanadium  Zrifluoride  with  MF. 
See  Fluovanadate,  M. 


VANADIUM  SULPHOCHLORIDE  SULPHUR  CHLORIDE 


1113 


Vanadium  hydride, 

Stable.     Does  not  react  with  boiling  H2O. 

Not  attacked  by  boiling  HC1.  but  oxidized 
by  hot  H2SO4. 

Sol.  in  boiling  HNO3.  (Muthmann,  A. 
1907,  356.  86.) 

Vanadium  ^hydroxide,  VO,  zH2O. 

Insol.  in  KOH  or  NaOH+Aq. 

V(OH)2.  Sol.  in  HC1.  (Locke  and  Ed- 
wards, Am.  Ch.  J.  1898,  20.  598.) 

Vanadium  tfnhydroxide,  V2O3,  zH2O. 

Easily  sol.  in  all  acids.  (Petersen,  J.  pr. 
(2)  40.  49.) 

Vanadium  te^rahydroxide  (Hypovanadic  hy- 
droxide), V2O2(OH)4+5H2O. 
Easily  sol.  in  acids  or  alkalies.      (Crow, 
Chem.  Soc.  30.  453.) 

Vanadium  Jniodide,  VI3+6H2O. 

Very  hydroscopic;  sol.  in  H2O.  Only  si. 
sol.  in  cold  cone.  HI+Aq. 

Sol.  in  alcohol.  (Piccini,  Z.  anorg.  1899, 
19.  399.) 

Vanadium  nitride,  V2N. 

Insol.  in  H2O,  HC1,  and  KOH+Aq.  Sol. 
in  HN03+H2S04. 

Decomp.  by  fusing  with  KOH.  (Muth- 
mann,  A.  1907,  366.  93.) 

Insol.  in  liquid  NH3.  (Gore,  Am.  Ch.  J. 
1898,  20.  830.) 

VN.     (Roscoe,  A.  suppl.  6.  114.) 

VN2.  Not  attacked  by  cold  HNO3+Aq. 
(Uhrlaub,  Pogg.  103.  134.) 

Vanadium  dioxide,  VO. 

Insol.  in  H2O;  easily  sol.  in  dil.  acids. 
(Roscoe,  A.  suppl.  6.  95.) 

Vanadium  Zrioxide,  V2O3. 

Oxidized  in  H2O  in  contact  with  air  and 
then  dissolves.  Insol.  in  acids,  except  HNO3, 
and  in  alkalies +Aq.  (Roscoe,  A.  suppl.  6. 
99  ) 

Easily  sol.  in  HF.  (Petersen,  J.  pr.  (2)  40. 
48.) 

Vanadium  te^roxide,  VO2. 

Sol.  in  acids  and  alkalies +Aq. 

Vanadium   pentoxide,   V2O6. 

Sol.  in  about  1000  pts.  H2O.     (Berzelius.) 

Sol.  in  acids,  alkali  hydrates,  and  carbon- 
ates +Aq.  Insol.  in  absolute,  very  si.  sol. 
in  dil.  alcohol. 

Insol.  in  glacial  HC2H3O2. 

Sol.  in  cone.  KF+Aq.  (Ditte,  C.  R.  106. 
1067.) 

Sol.  in  H2C2O4+Aq  and  alkali  oxalates  + 
Aq.  (Halberstadt,  Z.  anal.  22.  1.) 

Three  modifications. — (a)  Forms   hydrates 


with  2.  and  5H2O.  Sol.  in  H2O.  1  1.  of  sat. 
solution  contains  8  g.  V2O5. 

(/3)  V2O6,  2H2Q.  Very  si.  sol.  in  H2O.  1 1. 
of  sat.  solution  contains  0.5  g.  V2O6. 

(7)  V2O5,  5H2O.  Less  sol.  in  H2O  than 
£11.  H2O  contains  0.05  g.  V2O5  when  sat- 
urated. (Ditte,  C.  R.  101.  698.) 

See  Vanadic  acid. 

Vanadium  oxide,  V4O9=2VO2,  V2O5. 
See  Vanadate,  vanadium. 

V2O4,  V206+8/3H20.  (Brierley,  Chem. 
Soc.  49.  30.) 

See  also  Vanadiovanadic  acid. 
V2O<.  2V2O5+8H20. 
See  Vanadate,  vanadium. 

Vanadium  pentoxide  with  MF. 
See  Fluoxyvanadate,  M. 

Vanadium  oxy  compounds. 
See  Vanadyl  compounds. 

Vanadium  silicide,  V2Si. 

Insol.  in  H2O. 

Not  attacked  by  HC1,  HNO3  or  H2SO4. 
Readily  attacked  by  HF. 

Not  attacked  by  KOH+Aq,  NaOH+Aq 
or  NH4OH.  Decomp.  by  fused  KOH. 

Insol.  in  alcohol,  ether  and  benzene. 
(Moissan,  C.  R.  1902.  135.  496.) 

VSi2.  Sol.  in  HF;  insol.  in  acids  and  al- 
kalies. 

Decomp.  by  fused  KOH.  (Moissan,  C.  R. 
1902,  135.  78.) 

Vanadium  ^sulphide,  V2S2. 

Insol.  in  boiling  dij.  or  cone.  HC1,  dil. 
H2SO4+Aq,  or  cold  cone.  H2SO4.  Easily 
sol.  in  hot  dil.  or  cone.  HNO3+Aq,  or  in 
boiling  cone.  H2SO4.  Insol.  in  alkalies +Aq. 
SI.  sol.  in  KSH+Aq;  sol.  in  NH4SH+Aq. 
(Kay,  Chem.  Soc.  37.  728.) 

Vanadium  bisulphide,  V^a. 

Insol.  in  cold  HC1  or  dil.  H2SO4+Aq.  Very 
si.  sol.  in  hot  HC1  or  dil.  H2SO4+Aq.  More 
sol.  in  HNO3+Aq  or  cone.  H2SO4.  SI.  sol. 
in  NaOH  or  NH4QH+Aq.  Easily  sol.  in 
(NH4)2S  or  NH4SH+Aq,  also  in  K2S+Aq. 
(iCay,  Chem.  Soc.  37.  728.) 

Vanadium  pen  to  sulphide,  V2Se. 

SI.  attacked  by  hot  cone.  HC1  or  hot  dil. 
H2SO4+Aq;  sol.  in  hot  cone.  H2SO4.  Sol.  in 
hot  dil.  HNO3+Aq.  SI.  sol.  in  NH4OH+Aq, 
but  easily  dissolved  by  NaOH+Aq.  SI.  sol 
in  Na2S+Aq.  Sol.  in  NH4SH+Aq.  (Kay.) 

Vanadium   sulphochloride   sulphur  chloride, 

4VSC13,  S2C12. 

Decomp.  in  the  air.  (Koppel,  Z.  anorg. 
1905,  46.  357.) 


1114 


VANADOUS  ACID 


Vanadous  acid. 

Ammonium  vanadite,  basic.  2(NH4)2O, 

V204. 

SI.  sol.  in  cold,  easily  in  hot  H2O.  (Ditte, 
C.  R.  102.  1310.) 

Ammonium  vanadite,  (NH4)2V4O9+3H2O. 

Sol.  in  H2O.     (Crow,  Chem.  Soc.  30.  460.) 

+sH2O.    Sol.  in  H20. 

Insol.  in  alcohol,  ether  and  ammonia. 
(Koppel,  Z.  anorg.  1903.  36.  297.) 

+3H2O.  Easily  sol. 'in  H2O.  (Mawrow, 
Z.  anorg.  1907,  66.  150.) 

Barium  vanadite,  BaV4O9+4H2O. 

Ppt.     (Koppell,  Z.  anorg.  1903,  36.  300.) 
+5H2O.   Precipitate.    Easily  sol.  in  HNO3, 

or  HCl+Aq.     (Crow,  Chem.  Soc.  30.  460.) 

Lead  vanadite,  PbV409. 
.Ppt.     (Crow.) 

Potassium  vanadite,  K2V4O9+4H2O. 

Sol.  in  H2O. 

Insol.  in  alcohol,  ether  and  ammonia 
(Koppel,  Z.  anorg.  1903;  36.  300.) 

+7H2O.  Easily  sol.  in  H2O.  Insol.  in 
cold,  sol.  in  hot  KOH+Aq.  Insol.  in  alcohol. 
(Crow.) 

+H2O.    (Ditte.  C.  R.  102.  1310.) 

Silver  vanadite,  Ag2V4O9. 
Ppt.    (Crow.) 

Sodium  vanadite,  Na2V4O9-f4H2O. 

Sol.  in  H2O. 

Insol.  in  alcohol,  ether  and  ammonia. 
(Koppel,  Z.  anorg.  1903,  36.  299.) 

+7H2O.  Easily  sol.  in  H2O.  (Crow,  Chem. 
Soc.  30.  459.) 

Vanadosotungstic  acid. 

Ammonium  vanadosotungstate, 

5(NH4)2O,  2V2O4,  14WO8+13H2O. 
Very  sol.  in  H2O.     (E.  F.  Smith,  J.  Am. 
Chem.  Soc.  1903,  26.  1228.) 

Vanadous  acid. 

See  Hypovanadic  acid. 

Vanadovanadic  acid. 
See  Vanadicovanadic  acid. 

Vanadyl  bromide,  VOBr. 

Very  si.  sol.  in  H2O,  acetic  anhydride, 
ethyl  acetate,  and  acetone. 

Insol.  in  alcohol,  ether,  acetic  acid,  CHC13, 
toluene  and  CC14.  (Ruff,  B.  1911,  44.  2537.) 

Vanadyl  ^bromide,  VOBr3. 

Very  deliquescent,  and  sol.  in  H2O.  (Ros- 
coe.) 


Vanadyl  /n'bromide,  VOBr3. 

Very  deliquescent,  and  quickly  decomposes 
.n  moist  air.  Sol.  in  H2O.  (Roscoe.) 

Vanadyl  bromide,  V2O3Br2,  2HBr+7H2O. 
Very  deliquescent.    (Ditte,  C.  R .  102. 1310.) 

Vanadyl  seraichloride,  V2O2C1. 

Insol.  in  H2O.  Easily  sol.  in  HNO8+Aq. 
(Roscoe,  A.  suppl.  6.  114.) 

Vanadyl  raonochloride,  VOC1. 

Insol.  in  H2O.  Easily  sol.  in  HNO3+Aq. 
(Roscoe.) 

Vanadyl  ^chloride,  VOC12. 

Deliquescent.  Slowly  decomp.  by  H2O. 
Easily  sol.  in  HNO3+Aq.  (Roscoe.) 

Vanadyl  ^chloride,  VOC18. 

Deliquescent.    Sol.  in  H2O  and  alcohol  with 
decomp.     (Bedson,  A.  180.  235.) 
Sol.  in  ether  with  combination. 

Divanadyl  chloride,  V204C12+5H2O. 

Deliquescent,  and  sol.  in  H2O,  fuming 
HC1.  or  alcohol.  (Crow;  Chem.  Soc.  30.  457.) 

Vanadyl  chloride,  V2O3C12+4H20. 

Very  deliquescent.  (Ditte.  C.  R.  102. 
1310.) 

Vanadyl  platinum  chloride. 
See  Chloroplatinate,  vanadyl. 

Vanadyl  inchloride  ammonia,  VOC13,  #NH8. 

Decomp.  by  H2O.    (Roscoe.) 

Vanadyl  ^fluoride,  VOF2. 

Insol.  in  H2O.  Insol.  in  alcohol,  ether, 
CHC13.  SI.  sol.  in  acetone.  (Ruff,  B.  1911, 
44.  2546.) 

Vanadyl  Znfluoride,  VOF3. 

Very  hydroscopic.  Easily  sol.  in  H2O. 
Sol.  in  POC13  with  evolution  of  gas.  Diffi- 
cultly sol.  in  PC13  and  AsCl3.  Sol.  in  hot 
CHC13  and  acetic  anhydride.  (Ruff,  B.  1911, 
44.  2547.) 

Vanadyl  fluoride  wilh  MF. 

See  Fluoxyvanadate,  and  Fluoxhypovana- 
date,  M. 

Vanadyl  iodide,  V2O3I2,  3HI+10H2O. 

Very  deliquescent,  and  sol.  in  H2O.  (Ditte, 
C.  R.  102.  1310.) 

V203I2;2HI+8H2O.    As  above. 

Vanadyl  sulphide,  VOS  (?). 

(a)  Insol.  in  H2O,  alkalies,  alkali  sulphides 
+Aq.  Sol.  in  acids,  except  nitric  acid  and 
aqua  regia.  (Berzelius.) 


XANTHOCOBALTIC  MERCURIC  CHLORIDE 


1115 


(6)  Sol.  in  alkalies,  alkali  carbonates,  and 
sulphides+Aq.  Insol.  in  acids.  (Berzelius.) 

Water,  H2O. 

Water  is  the  most  universal  solvent.  It 
absorbs  all  gases,  usually  with  an  increase  of 
volume,  seldom,  as  in  the  case  of  NH3,  with 
a  diminution  of  volume.  It  dissolves  almost 
all  solids  in  greater  or  less  quantity,  and 
mixes  with  or  dissolves  considerable  amounts 
of  many  liquids. 

Miscible  with  alcohol.    Sol.  in  36  pts.  ether. 

Sol.  in  30-33  vols.  ethyl  acetate.    (Becker.) 

Sol.  in  5  vols.  iodhydrin. 

SI.  sol.  in  most  of  the  fatty  oils. 

Solubility  in  organic  solvents  at  t°. 


G.  H2O  in 

Solvent 

t° 

100  g.  of  the 
solution 

Benzene 

+3 

0.030 

23 

0.060 

40 

0.114 

55 

0.184 

66 

0.255 

77 

0.337 

Petroleum 

-2 

0.0012 

bpt.  190-250° 

+  18 

0.005 

at  atmos.  pressure 

23 

0.007 

30 

0.008 

36 

0.012 

53 

0.026 

59 

0.031 

61 

0.035 

66 

0.043 

79 

0.063 

85 

0.075 

94 

0.097 

Paraffin  oil 

+  16 

0.003 

bpt.  200-300° 

50 

0.013 

at  10  mm  .  pressur 

65 

0.022 

73 

0.030 

77 

0.035 

94 

0.055 

(Groschuff,  Z.  Elektrochem,  1911,  17.  350.) 

White  precipitate,  fusible. 

See  Mercuricfo'ammonium  chloride. 

White  precipitate,  infusible. 
See  Mercuric  chloramide. 

Xanthochromium  bromide, 

Cr(NO2)(NH3)5Br2. 

Sol.    in    H2O.      Resembles    the    chloride 
(Christensen,  J.  pr,.'  (2)  24.  74.) 

—  carbonate,  dr(Kp2)(NH,)6CO,. 

Easily  sol.  in  H2O.  -(Christensen.) 


Xanthochromium  chloride, 

Cr(N02)(NH3)6Cl2. 

More  sol.  in  H2O  than  the  roseo,  but  less 
than  the  purpureo  salt. 

Solution  decomp.  by  light  or  boiling.  De- 
comp.  by  dil.  acids.  Sol.  in  NaOH+Aq  and 
n  NH4OH+Aq  (sp.  gr.  0.91).  Insol.  in 
alcohol.  (Christensen,  J.  pr.  (2)  24.  74.) 

—  chloroplatinate,  Cr(NO2)(NH3)5PtCl6. 

Insol.  in  pure  H2O,  but  sol.  when  warmed 
with  H2O  containing  HC1,  with  formation  of 
a  new  double  salt.  (Christensen.) 

—  mercuric  chloride,  Cr(NO2)(NH3)6Cl2j 

2HgCl2. 

Precipitate.  Decomp.  by  long  contact  with 
H2O.  (Christensen.) 

—  chromate,  Cr(N02)(NH8)6CrO4. 
Difficultly  sol.  in  H2O.    (Christensen.) 

—  bichromate,  Cr(N02)(NH3)6Cr2O7. 
Difficultly  sol.  in  H2O.    (Cliristensen.) 

—  dithioriate,  Cr(NO2)(NH3)6S2O6. 
Insol.  in  cold  H2O.    (Christensen.) 

hydroxide,   Cr(N02)(NH3)6(OH)2. 

Known   only  in   solution.      (Christensen.) 

—  iodide,  Cr(NO2)(NH3)5I2. 

Quite  difficultly  sol.  in  H2O.    (Christensen.) 

—  nitrate,  Cr(NO2)(NH3)6(N03)2. 

Sol.  in  about  150  pts.  H2O.    (Christensen.) 

—  sulphate,  Cr(NO2)(NH3)5SO4+H2O. 
Sol.  in  H2O  and  (NH4)2SO4+Aq.     (Chris- 
tensen.) 

Xanthocobaltic  bromide, 

Co(NH3)6(NO2)Br2. 

Easily  sol.  in  cold  H2O.  (Werner  and 
Miolati,  Gazz.  ch.  it.  23,  2.  140.) 

—  bromonitrate,  Co(NO2)(NH3)6(NO3)Br. 
SI.  sol.  in  cold,  more  easily  in  hot  H2O. 

(Gibbs.) 

•  chloride,  Co(NO2)(NH3)6Cl2. 

SI.  sol.  in  cold  H2O,  and  decomp.  by  boiling 
therewith.  Insol.  in  HCl+Aq  and  alkali 
chlorides +Aq.  Easily  decomp.  by  boiling 
with  acids,  even  dilute.  (Gibbs  and  Genth.) 

Sol.  in  50  pts.  cold  H2O.  (Jorgensen,  Z. 
anorg.  6.  172.) 

.  mercuric  chloride,  Co(NO2)(NH3)6Cl2, 

2HgCl2+H20. 

Insol.  in  cold,  sL  sol.  in  hot  H2O  without 
decomp.  More  sol.  in  acidified  H2O.  (Gibbs 
and  Genth.) 


1116 


XANTHOCOBALTIC  CHLORAURATE 


Xanthocobaltic  chloraurate, 

Co(NO2)(NH3)5Cl2,  AuCl3+H2O. 
Can  be  easily  crystallised  out  of  hot  H2O. 
(Gibbs  and  Genth,  Sill.  Am.  J.  (2)  24.  90.) 

chloronitrate,  Co(NO2)(NH3)5(NO3)Cl. 

SI.  sol.  in  cold;,  more  easily  in  hot  H2O. 

chloronitrate  gold  chloride, 

Co(N02)(NH3)5(N03)Cl,  AuCl3. 

chloronitrate  platinic  chloride, 

2Co(NO2)(NH3)6(NO3)Cl,  PtCl4. 

chloroplatinate,  Co(NO2)(NH3)6Cl2, 

PtCl4+H20. 

Scarcely  sol.  in  hot  or  cold  H20.  Can  be 
recryst.  from  dil.  HNQa+Aq.  Sol.  in  hot  dil. 
HCl+Aq.  (Gibbs  and  Genth,  Sill.  Am.  J.  (2) 
24.  91.) 

chromate,  Co(NO2)(NH3)6CrO4+H2O. 

Very  si.  sol.  in  cold,  and  but  slightly  sol.  in 

hotH2O.    (Gibbs.) 

bichromate,  Co(NO2)(NH3)5Cr2O7. 

Easily  sol.  in  hot  H2O. 

ferrocyanide,  [Co(NO2)(NH3)6]2Fe(CN)6 

+7H20. 

Nearly  insol.  in  cold,  decomp.  by  warm 
H2O. 

+6H2O.    (Braun,  A.  132.  47.) 

iodide,  Co(N02)(NH3)5I2. 

Sol.  in  H2O.    (Gibbs.) 

iodosulphate, 

[Co(NO2j(NH3)5]2(SO4)I2. 
Sol.  in  H2O. 

periodosulphate, 

[Co(N02)(NH3)6]2(S04)l4. 
Easily  decomp.  by  hot  H2O. 

nitrate,  Co(NO2)(NH3)6(NO3)2. 

SI.  sol.  in  cold,  moderately  sol.  in  hot  H2O. 
Decomp.  by  boiling.  Much  less  sol.  than 
NH4C1  or  (NH4)2SO4  in  cold  H2O.  Insol.  in 
HNO3.  (Gibbs  and  Genth.) 

nitrite,  Co(N02)(NH3)5(N02)2+2H20. 

Sol.  inH2O.    (Gibbs.) 

cobaltic  nitrite,  Co(NO2)(NH3)5(NO2)2 

+2H20. 

SI.  sol.  in  H2O.  (Gibbs,  Proc.  Am.  Acad. 
11.  8.) 

Is  nitratopurpureocobaltic  cobaltic  nitrite, 


[(NO3)Co(NH3)8j3[Co(NO2)6]2+2H2O.      (Jor- 
gensen, Z.  anorg.  6.  175.) 

[Co(NO2)(NH3)5]3[Co(NO2)6]2.  Not  so 
difficultly  sol.  as  the  luteo  salt.  (Jorgensen.) 

Xanthocobaltic  famine  cobaltic  nitrite, 

Co2(N02)2(NH3)io[Co2(NH3)4(NO2)8]2. 

Can  be  recryst.  from  hot  H20.  (Gibbs, 
Proc.  Am.  Acad.  11.  8.) 

=  (N02)Co(NH3)6[(Np2)2(NH3)2Co(N02)2]2. 
Xanthocobaltic  famine  cobaltic  nitrite. 
Very  si.  sol.  in  cold  H2O.  (Jorgensen,  Z. 
anorg.  5.  180.) 

—  oxalate,  Co(NO2)(NH3)6C2O4, 

Nearly  insol.  in  cold,  si.  sol.  in  hot  H2O. 

_  sulphate,    Co(NO2)(NH3)5SO4. 

Moderately  sol.  in  hot,  much  less  in  cold 
H2O.  Sol.  without  decomp.  in  H2SO4+Aq. 
(Gibbs  and  Genth.) 

Sol.  in  25  pts.  hot  H2O  acidified  with 
HC2H3O2.  (Jorgensen,  Z.  anorg.  6.  172.) 

4Co(NO2)(NH3)5SO4,  3H2SO4.  Decomp. 
by  H2O,  not  by  absolute  alcohol.  (Jorgensen.) 

Xanthorhodium  bromide, 

(NO2)Rh(NH3)5Br2. 

Moderately  sol.  in  H2O.  (Jorgensen,  J. 
pr.  (2)  34.  394.) 

-chloride,  (NO2)Rh(NH3)6Cl2. 

Much  more  sol.  in' H2O  than  the  nitrate. 

-  chloroplatinate,  (NO2)Rh(NH3)5PtCl6. 
Ppt.    Extremely  si.  sol.  in  cold  H2O. 

dithionate,  (NO2)Rh(NH3)5S2O6+H2O. 


Nearly  insol.  in  H2O. 

fluosilicate,   (NO2)Rh(NH3)5SiF6. 

Ppt. 

hydroxide,   (NO2)Rh(NH3)5(OH)2. 

—  nitrate,   (N02)Rh(NH3)6(NO3)2. 

Moderately  sol.  in  cold,  easily  in  hot  H2O. 
Insol.  in  alcohol.  Less  sol.  in  cone.  NH4OH  + 
Aq  than  in  H2O. 

Insol.  in  dil.  HNO3+Aq;  sol.  in  HNO3+Aq 
of  1.4  sp.  gr. 

oxalate,  (NO2)Rh(NH3)6C2O4. 

Nearly  insol.  in  cold  H2O.  Very  si.  sol.  in 
warm  H20.  Easily  sol.  in  dil.  HC2H3O2+Aq. 

sulphate,  (NO2)Rh(NH3)6SO4. 

Slowly  sol.  in  cold,  quite  easily  in  hot  H2O. 

4(NO2)Rh(NH3)5SO4,  3H2SO4.  SI.  sol.  in 
cold,  easily  in  hot  H2O.  Can  be  recrystal- 
lized  from  dil.  H2SO4+Aq. 


ZINC 


1117 


Xenon,  Xe. 

Absorption  by  H2O  at  t°. 


t 

Absorption  -coefficient 

0 
10 
20 
30 
40 
50 

0.2189 
0.1500 
0.1109 
0.0900 
0.0812 
0.0878 

(Antropoff,  Roy.  Soc.  Proc.  1910,  83.  A,  480.) 
Ytterbium,  Yb. 

Ytterbium  bromide,  YbBr3+8H2O. 

Very  sol.  in  H2O.  Hydroscopic.  (Cleve, 
Z.  anorg.  1902,  32.  135.) 

Ytterbium  chloride,  YbCl3+6H2O. 

Very  sol.  in  H2O.  (Cleve,  Z.  anorg.  1902, 
32.  134.) 

Mpt.  150-155°.  Anhydrous  salt  is  sol.  in 
H2O  and  in  alcohol.  (Matignon,  A.  ch.  1906, 
(8)  8.  442.) 

Ytterbium  oxide,  Yb2O3. 

Slowly  attacked  by  cold  or  warm  acids, 
but  easily  sol.  at  100°. 

Ytterbium  oxychloride,  YbOCl. 

Ppt.    (Cleve,  Z.  anorg.  1902,  32.  135.) 

Yttrium,  Y. 

Decomposes  H2O.  (Cleve,  Bull.  Soc.  (2) 
21.  344.)  Decomp.  H2O  slightly  at  ord.  temp., 
more  rapidly  by  boiling.  Easily  sol.  in  dil. 
acids,  even  acetic  acid.  Slightly  acted  upon 
by  cone.  H2SO4.  Decomposes  hot  KOH-f-Aq 
and  cold  NH4Cl+Aq.  Not  attacked  by 
NH4OH+Aq.  (Popp,  A.  131.  179.) 

Popp's  yttrium  contained  erbium. 

Yttrium  bromide,  YBr3. 

Sol.  in  H2O  with  evolution  of  heat.  (Du- 
boin,  C.  R.  107.  243.) 

+9H2O.  Deliquescent.  Easily  sol.  in  H2O 
and  alcohol.  Insol.  in  ether.  (Cleve.) 

Yttrium  carbide,  YC2. 

Decomp.  by  H2O  and  by  dil  acids;  very 
slowly  attacked  by  cone,  acids.  (Moissan, 
C.  R.  1896,  122.  575.) 

Decomp.  by  H2O  and  dil.  acids.  (Petters- 
son,  B.  1895,  28.  2421.) 

Yttrium  chloride,  YC13. 

Anhydrous.  Sol.  in  H2O  with  evolution  of 
heat.  (Cleve.) 

+6H2O.  Deliquescent.  Very  sol.  in  H2O. 
SI.  sol.  in  alcohol.  Insol.  in  ether.  (Cleve.) 

Mpt.  156-160°;  sol.  in  alcohol. 


60.1  grams  anhydrous  salt  are  sol.  in 
100  grams  of  abs.  alcohol  at  15°. 

6,5  grams  are  sol.  in  100  grams  pyridine. 
(Matignon,  A.  ch.  1906,  (8)  8.  437.) 

Yttrium  fluoride,  YF3+^H2O. 

Nearly  insol.  in  dil.  acids.     (Cleve.) 

Yttrium  hydroxide,  Y2O3,  6H2O  or  Y2O6H6-f 
3H2O. 

Insol.  in  H2O. 

Insol.  in  KOH  or  NaOH+Aq.  Easily 
sol.  in  acids.  Sol.  in  alkali  carbonates +Aq. 
When  freshly  pptd.,  easily  sol.  in  NH4C1+ 
Aq. 

Yttrium  iodide,  YI3. 

Very  deliquescent.  Easily  sol.  in  H2O  and 
alcohol. 

SI.  sol.  in  ether.     (Cleve.) 

Yttrium  oxide,  Y203. 

Insol.  in  H2O.  SI.  sol.  in  cold  HC1,  HNO3, 
or  dil.  H2SO4+Aq,  but  gradually  completely 
sol.  on  warming.  Insol.  in  NH4OH  and  si. 
sol.  in  KOH+Aq.  Sol.  in  HC2H3O2+Aq. 
Somewhat  sol.  in  K2CO3+Aq. 

Yttrium  peroxide,  Y4O9. 

(Cleve,  Bull.  Soc.  (2)  43.,  53.) 

Yttrium  oxychloride,  Y2O2C12. 
Insol.  in  H2O.     (Popp.) 

Yttrium  sulphide,  Y2S3. 

Not  prepared  in  pure  state.  Impure  is 
insol.  in  H2O,  and  partially  decomp.  thereby. 
Easily  sol.  in  acids  with  decomp.  (Popp.) 

Zinc,  Zn. 

Not  attacked  by  pure  cold  H2O.  Slowly 
oxidised  by  boiling  H2O.  Pure  H2O  free  from 
O  dissolved  nothing  from  2500  sq.  mm.  Zn. 
Presence  of  air  containing  CO2  caused  a  solu- 
tion of  3.5  mg.  Zn,  which  maximum  was 
reached  in  2  days.  Air  without  CO2  also 
caused  a  slight  action.  (Snyders,  B.  11.  936.) 

100  ccm.  distilled  H2O  dissolved  14  mg.  Zn 
from  11.8  sq.  cm.  in  one  week,  during  which 
air  free  from  CO2  was  passed  through  the 
liquid,  and  19  mg.  when  air  containing  CO2 
was  used.  (Wagner,  Dingl.  221.  260.) 

Filtered  rain  water  was  found  to  contain 
20  mg.  Zn  per  1.  (Burg,  Isis,  1873.  119.) 

Very  pure  H2O,  when  conducted  through 
a  great  length  of  galvanized  iron  pipe,  con- 
tained 1.7  pts.  Zn  to  100,000  pts.  H2O. 
(Davies,  J.  Soc.  Chem.  Ind.  1899,  18.  102.) 

Action  of  H2O  on  Zn  in  galvanized  pipes 
is  caused  by  electrolysis.  (Smetham,  C.  N. 
1879,  39.  236.) 

All  kinds  of  H2O  attack  Zn,  rain  water  the 
least. 

In  distilled  H2O  exposed  to  air  Zn  is  abun- 


1118 


ZINC 


dantly  coated  with  ZnCO3,  2ZnO+3H2O.  By 
allowing  32  g.  Zn  to  stand  in  270  cc.  distilled 
H2O  in  a  flask  loosely  stoppered  with  filter 
paper,  1.2  pts.  Zn  to  100,000  pts.  H2O  was 
found  in  solution  in  1-2  days.  (Smith,  J.  Soc. 
Chem.  Ind.  1904,  23.  475.) 

Sol.  in  all  acids.  Very  slowly  sol.  in  dil, 
HC1  or  H2SO4+Aq  in  glass  vessels  if  Zn  is 
pure.  According  to  Jacquelain,  24  hours  were 
necessary  to  dissolve  6  g.  pure  tfinc.  When 
fused  at  the  lowest  possible  temperature,  it  is 
much  more  slowly  sol.  than  when  heated  to  a 
red  heat.  In  both  cases  it  is  much  more 
rapidly  dissolved  if  cooled  quickly.  (Bolley, 
A.  96.  294;  Rammelsberg.) 

Dil.  H2SO4+Aq  dissolves  given  %  zinc  in  the 
same  length  of  time  (B=  according  to 
Bolley,  R  — according  to  Rammelsberg) 


Slowly  cooled      Rapidly  cooled 

B                   R          B 

R 

Cast  at  the  melt- 

ing point             42  .  5      74  .  1    13  .  0 

0.9 

Cast  at  a  red  heat  100.0       69.4    85.5 

9.5 

50  ccm.  H2SO4+Aq  dissolved  in  2  hours 

the 

following  amts.  from  1  sq.  cm.  Zn  at  t°. 

t° 

Strength  of  acid 

Grms.  dissolved 

20 

H2SO4 

0.000 

130 

n 

0.075 

150 

a 

0.232 

20 

H2SO4+H2O 

0.002 

130 

u 

0.142 

150 

« 

0.345 

20 

H2SO4+2H20 

0.002 

130 

« 

4.916 

150 

" 

5.450 

20 

H2SO4+3H2O 

0.005 

130. 

« 

3.080 

20 

H2SO4+4H2O 

0.049 

130 

u 

0.456 

20 

H2SO4+5H2O 

0.027 

130 

u 

0.337 

20 

H2SO4+6H2O 

0.018 

100 

" 

3.16 

(Calvert  and  Johnson,  Chem.  Soc.  19.  437.) 

C.  P.  zinc  is  more  quickly  sol.  in  dil.  acids 
in  vacuo  than  under  normal  pressure,  the 
ratio  being  about  1 : 6.5.  The  rate  of  solubil- 
ity increases  slowly  with  rise  of  temp,  from 
0°  to  98°,  when  it  amounts  to  about  4  times 
that  at  0°,  but  from  98°-100°  the  increase  is 
thirteenfold.  Thus,  as  an  average  of  6  ex- 
periments,, dil.  H2SO4+Aq  (1:20)  dissolves  in 
30  minutes  2.1  mg.  Zn  at  0°;  4.9  mg.  at  20°  • 
7.4  mg.  at  60°;  9.3  mg.  at  98°;  but  122.1  mg! 
at  100°.  If,  however,  the  acid  was  prevented 
from  boiling  by  increasing  the  pressure,  the 
sudden  increase  between  98°  and  100°  does 
not  take  place. 


The  rate  of  solubility  in  dil.  H2SO4+Aq 
(1 :  20)  is  also  increased  175  times  by  the  addi- 
tion of  CrO3  and  306  times  by  the  addition 
of  H202.  The  above  phenomena  are  ex- 
plained by  assuming  the  formation  of  a 
condensed  hydrogen  atmosphere  around  the 
metal,  which  prevents  the  further  action  of 
the  acid.  (Weeren,  B.  24.  1785.) 

Not  attacked  by  HNO3+Aq  of  1.512  to 
1.419  sp.  gr.  at  a  temp,  of  —18°  or  less,  but 
violently  attacked  if  temp,  is  raised.  HNO3  + 
Aq  of  1.419-1.401  sp.  gr.  does  not  attack  Zn 
at  temp,  of  a  freezing  mixture,  but  violently 
at  0°.  More  dil.  HNO3+Aq  attacks  Zn  even 
at  —20°.  (Millon,  A.  ch.  (3)  6.  99.) 

Sol.  in  H2CO3+Aq.     (Berzelius.) 

Solubility  of  Zn  in  acids  is  very  much 
affected  by  the  presence  of  small  quantities 
of  various  metallic  salts.  Small  amts.  of 
PtCl4+Aq  accelerated  the  action  of  H2SO4+ 
Aq  149  times,  and  As2O3  123  times.  HgCl2 
has  a  strong  retarding  action  owing  to  pptn. 
of  Hg  on  the  Zn. 

The  rate  of  solution  of  Zn  in  acids  and  the 
effect  of  changes  in  concentration  and  tem- 
perature and  of  the  presence  of  inorganic 
salts  and  organic  substances  on  this  rate  has 
been  studied.  26  Tables  are  given.  (Ericson- 
Aure*n,  Z.  anorg.  1901,  27.  209-253.)  . 

Speed  of  solution  in  H2SO4  and  in  HC1. 
(Centnerszwer,  Z.  phys.  Ch.  1914,  87.  692.) 

Various  saline  solutions  have  a  strong  sol- 
vent power  in  presence  of  PtCl4,  i.e.  KC1, 
NaCl,  Na2S04,  K2SO4,  MgSO4+Aq.  PtCl4 
also  causes  Zn  to  decompose  distilled  H2O. 
CuSO4  hae  a  similar  but  less  energetic 
effect. 

In  all  the  above  cases  the  disengagement  of 
hydrogen  is  slower  in  the  dark  than  in  the 
light.  (Millon,  C.  R.  21.  37.) 

According  to  Barreswill  (C.  R .  21.  292)  the 
above  reactions  are  all  caused  by  galvanic 
action  due  to  pptd.  metal,  and  a  piece  of  Pt 
in  contact  with  the  Zn  causes  the  same  action 
as  the  PtCl4  in  solution. 

Easily  sol.  in  alkalies +Aq,  even  NH4OH+ 
Aq,  especially  when  the  Zn  is  in  contact  with 
Fe.  Sol.  m"NaCl-fAq  with  pptn.  of  ZnO. 
(Siersch,  J.  B.  1867.  257.) 

Sol.  in  sat.  alkali  and  alkali-earth  chlorides 
+Aq.  (Post,  1872.) 

Sol.  in  NH4  salts+Aq.  (Lorin,  J.  B.  1865. 
124.) 

Sol.  in  sat.  Na2SO4,  K2SO4,  MgSO4,  NaNO3, 
KNO3,  Ba(NO3)2,  CaCl2,  MgCl2,  and 
NH4NO3+Aq.  Chlorides  and  sulphates 
(especially  Na2SO4  and  MgCl2)  have  strong- 
est action,  MgSO4  and  nitrates  the  least.  The 
action  was  greatly  increased  by  heat.  (Sny- 
ders,  B.  11.  936.) 

Sol.  in  boiling  NH4Cl+Aq.  Sol.  in  neutral 
FeCl2+Aq  with  pptn.  of  Fe,  especially  easily 
at  100°.  (Capitaine,  C.  R.  9.  737.) 

Sol.  in  NiSO4+Aq  with  pptn.  of  NiO. 
(Tupputi.) 

Sol.  in  cone,  hot  ZnCl2+Aq,  but  Zn  oxy- 


ZINC  BROMIDE 


1119 


chloride  is  pptd.  on  diluting.     (Ordwav,  Am. 
J.  Sci.  (2)  23.  222.) 

Sol.  in  GlSO4+Aq.     (Debray.) 

Solubility  of  Zn  in  dilute  solutions  of  salts: 
100  ccm.  of  solutions  of  the  given  salts 
were  allowed  to  act  one  week  on  11.8  sq. 
cm.  Zn  while  a  current  of  air  with  or 
without  CO2  was  passed  through  the 
solution. 


Salt 

G.   salt 
in  100  ccm. 
solution 

Mg.   Zn 
dissolved 
without  CO2 

Mg.  Zn 
dissolved 
with  COz 

NaCl  } 

or 

0.5 

7 

38 

KC1    J 

NH4C1 

1.0 

51 

36 

MgCl2 

0.83 

18 

54 

K2SO4 

1.0 

30 

53 

KNO3 

1.0 

9 

37 

Na2CO3 

1.0 

13 

NaOH 

0.923 

60 

CaO2H2 

Sat 

3 

(Wagner,  Dingl.  221.  260.) 

Action  of  dil.  salt  solutions  (1%)  on  Zn.  The 
following  amts.  of  Zn  in  mg.  were  dis- 
solved from  2500  sq.  mm.  Zn  in  14  days 
by  400  ccm.  1%  solution  of  the  given 
salts : 


Violently  decomp.  by  dil.  HC1  or  H2SO4+Aq, 
also  by  HNO3+Aq.  Completely  sol.  in  HC1 
+Aq  mixed  with  a  little  HNO3.  (Cooke.) 

Zinc  azoimide,  basic,  Zn(OH)N8. 

Very  si.  sol.  in  H2O.  Decomp.  by  hot 
H2O.  (Curtius,  J.  pr.  1898,  (2)  68.  293.) 

Zinc  azoimide  ammonia,  ZnN6,  2NH8. 

Insol.  in  H2O,  but  gradually  decomp. 
thereby.  (Dennis,  J.  Am.  Chem.  Soc.  1907 
29.  20.) 

Zinc  bromide,  ZnBr2. 

Very  deliquescent,  and  sol.  in  H2O. 

Sat.  ZnBr2+Aq  contains  at: 
—20°       +4°       22°        97° 
66.3        68.8      77.5      83.6%ZnBr2, 

107°        170°       210°      375°  (mpt.) 
83.8        85.0      89.3      100%  ZnBr2. 
(Etard,  A.  ch.  1894,  (7)  2.  541.) 

Solubility  in  H2O. 

100  g.  of  the  sat.  solution  contain  at: 
35°        40°        60°        80°       100° 
85.45   85.53   86.08    86.57    87 . 05  g.  ZnBr2. 
(Dietz,  Z.  anorg.  1899,  20.  250.) 


Salt 

Mg.  Zn 

Salt 

Mg.  Zn 

Sp.  gr.  of  ZnBr2+Aq  at  19. 

5°  containing 

NaCl    . 
KC1      .      . 

CaCl2   .      . 

11.2 
14.8 
15.2 

NaNO3 
Ba(NO,),   .      . 
NH4C1        .      . 

6 
8 
24.0 

18.3 
1  .  1849       ] 

31.7 
.3519 

43.2  %  ZnBr2, 
1.5276 

MgCl2  .      . 
BaCl2   .      . 
K2SO4 
MgSO4       . 

17.2 
13.2 
12.0 

8.8 

(NH4)2SO4   ... 
NH4N03     .      . 
NaHCO,    .     . 
K2CO3        .      . 

31.6 
26.0 
0 
0 

52.6           59.1             68     %  ZnBr2. 
1.7082       1.8525       2.1027 
(Kremers,  Pogg.  108.  117.) 

KNO3 

6.8 

Na2CO3      .      . 

0 

Sn  jrr.  of  ZnBr9+Aa  at  19.5°. 

SI    attacked  by  H2O  at  80°,  bv  hot  cone. 
NH4OH;  attacked  by  H3PO4  or  NaCl+Aq; 

ZnBr2 

Sp.  gr. 

ZnBr2 

Sp.  gr. 

% 

ZnBr2 

Sp.  gr. 

very  si.  attacked  by  NaNO3+Aq  or  KNO3  + 
Aq  at  100°.    (Smith,  J.  Soc.  Chem.  Ind.  1904, 
23    476  ) 

5 

10 

1.045 
1.093 

25 
30 

1.265 
1.330 

45 
50 

1.560 
1.650 

%  ccm.  oleic  acid  dissolves  0.0210  g.  Zn 

15 

1.196 

35 

1.400 

55 

1.755 

in  6  days.     (Gates,  J.  phys.  Chem.  1911,  16. 

20 

1.204 

40 

1.475 

60 

1.875 

Attacked    by    cane    sugar  +Aq    at    115° 

(Kremers,  calculated  by  Gerlach,  Z.  anal.  8. 

(Klein  and  Berg,  C.  R.  102.  1170.) 

285.) 

Zinc  amide,  Zn(NH2)2. 

Decomp.  by  H2O  and  alcohol.  Insol.  in 
ether.  (Frankland,  Phil.  Mag.  (4)  15.  149.) 

Zinc  antimonide,  ZnSb. 

Does  not  decomp.  boiling  H2O  except 
slightly.  Not  attacked  by  dil.  mineral  acids 
but  decomp.  by  cone.  HC1  or  HNO3+Aq 
(Cooke,  Proc.  Am.  Acad.  6.  348.) 

Zn3Sb2.     Decomp.   H2O   rapidly  at   100 


Sol.  in  cone.  HC1  or  HC2H3O2+Aq,  also 
in  NH4OH+Aq. 

Sol.  in  AlBr3.  (Isbekow,  Z.  anorg.  1913. 
84  27  ) 

Very  si.  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  830.) 

Sol  in  alcohol  and  ether.  (Berthemot,  J. 
Pharm.  14.  610.) 

Sol  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 


1120 


ZINC  BROMIDE  AMMONIA 


Insol.  in  ethyl  acetate.  (Naumann,  B. 
1910,  43.  314.) 

More  sol.  in  anhydrous  ether  than  in  abs. 
alcohol.  Insol.  in  CS2.  (Hampe,  Ch.  Z. 
1887,  11.  846.) 

Sol.  in  quinoline.  (Beckmann  and  Gabel. 
Z.  anorg.  1906,  61.  236.) 

Mol.  weight  determined  in  pyridine. 
(Werner,  Z.  anorg.  1897,  16.  22.) 

+H2O.     (Lescoeur,  A.  ch.  1894,  (7)  2.  78.) 

-j-2H2O.    Very  hygroscopic. 

Solubility  in  H2O. 

100  g.  of  the  sat.  solution  contain  at: 
—8°      0°         13°     25°      30°      37°(mpt.) 
79.06  79.55  80.76  82.46  84.08  86.20  g.  ZnBr2. 
(Dietz,  Z.  anorg.  1899,  20.  250.) 

+3H2O.     Solubility  in  H2O. 

100  g.  of  the  sat.  solution  contain  at: 
—15°         —10°  —5°  (mpt.) 

77 .13        78 . 45        80 . 64  g.  ZnBr2. 
(Dietz,  Z.  anorg.  1899,  20.  250.) 


ammonia, 


Zinc  bromide 

Decomp.  by  H2O 
easily   in 
berg,  Pogj 


ZnBr2,  2NH3. 
SI.  sol.  in  cold,  more 
warm    NH4OH+Aq.      (Rammels- 
;.  65.  240.) 

).     Decomp.  by  H2O  with  separa- 
tion of  ZnO.    (Andre;  C.  R.  96.  703.) 

+H2O.  Above  salt  of  Rammelsberg's 
has  this  composition.  (Andre*.) 

3ZnBr2,  8NH3+2H2O.  Decomp.  by  H2O. 
(Andre".) 

3ZnBr2,  10NH3+H2O.  Decomp.  by  H2O. 
(Andre-.) 

2ZnBr2.  10NH3.  Efflorescent.  Decomp. 
by  H2O.  '  (Andre*.) 

Zinc  bromide  cupric  oxide,  ZnBr2,  3CuO-f 

2H2O. 
+4H2O.    (Mailhe,  C.  R.  1901, 133.  227.) 

Zinc  bromide  hydrazine,  ZnBr2,  2N2H4. 

Decomp.  by  H2O. 

Sol.  in  NH4OH+Aq.  (Franzen,  Z.  anorg. 
1908,  60.  277.) 

Zinc  chloride,  ZnCl2. 

Very  deliquescent,  and  sol.  in  H2O. 

Sol.  in  0.333  pt.  H2O  at  18.75°.     Abl.) 
ZnCh+Aq    sat.    at    12.5°    contains    78.5%    ZnCl2. 
(Hassenfratz,  A.  ch.  28.  291.) 

Solubility  in  H2O. 

100  g.  of  the  sat.  solution  contain  at: 
15°       20°       41°       60°       100° 
79.12  81.19  82.21  83.51  86.01  g.  ZnCl2. 
(Dietz,  Z.  anorg.  1899,  20.  245.) 

ZnCl2+Aq  containing  1  pt  ZnCl2  in  1.8205 
pts.  H2O  at  18°  has  sp.  gr.  =  1.3666.  (Hit- 
torf,  Z.  phys.  Ch.  1902,  39.  628.) 


Solubility  in  H2O  at  t°. 
100  g.  H2O  dissolve  g.  ZnCl2. 


t° 

Solid  phase 

ZnCl2 

—  5 

ice 

14 

—  10 

25 

—  40 

" 

83 

-62 
—  50 

ice:4aq 
ZnCl2+4H20 

104 
113 

'  cryohydrate  point 

—  40 

127 

—  30 

4aq:3aq 

160 

transition  point 

-10 

ZnCl2+3H20 

189 

0 

" 

208 

+5 

" 

230 

6.5 

" 

252 

mpt. 

5 

" 

282 

0 

3aq:lKaq 

309 

eutectic  point 

0 

ZnCl2  +2  J^H2O 

235 

6.5 

2>£aq:3aq 

252 

transition  point 

10 

ZnCls  +2^H2O 

272 

12.5 

" 

303 

mpt. 

11.5 

2^aq:l^aq 

335 

eutectic  point 

9 

2^aq:laq 

360 

eutectic  point 

6 

ZnCl2  +2^H2O 

385 

-6 

ZnCl2+lHH2O 

298 

+  10 

" 

330 

20 

M 

368 

26 

13^aq:laq 

423 

transition  point 

26.3 

l>iaq:ZnCl2 

433 

transition  point 

0 

ZnCl2+H20 

342 

10 

364 

20 

" 

396 

28 

laq:ZnC!2 

436 

transition  point 

31 

ZnCl2+H20 

477 

25 

ZnCh 

432 

40 

" 

452 

60 

" 

488 

80 

" 

543 

100 

.•    '        " 

615 

262 

mpt. 

(Mylius  and  Dietz,  Z.  anorg.  1905,  44.  217.) 
See  also  below  under  hydrated  salts. 

Sp.  gr.  of  ZnCl2+Aq  at  19.5°. 


%  ZnCl2 

Sp.  gr. 

%  ZnCh 

Sp.  gr. 

1.3859 
1.5551 

13.8 

25.8 

1  .  1275 
1.2466 

37.5 
49.2 

CKremers,  Fogg.  106.  360.) 
Sp.  gr.  of  ZnCl2+Aq  at  19.5°. 

%  ZnCh 
1 

5 
10 
15 
20 

Sp.  gr. 

1.010 
1.045 
1.091 
1.137 
1.186 

7o  ZnCh 

Sp.  gr. 

%  ZnCh 

Sp.  gr. 

25 
30 
35 
40 

1.238 
1.291 
1.352 
1.420 

45 
50 
55 
60 

1.488 
1.566 
1.650 
1.740 

(Gerlach,   Z.   anal.   8.   283,    calculated  from 
Kremers.) 

Sp.  gr.  of  ZnCl2+Aq  at  t°. 

t°                    15°           15°           15°  15° 

£ZnCl2          2.5        4.89        10.0  20.0 

p.gr.           1.024       1.046       1.094  1.190 

t°  15°  15°  15° 

%ZnCl2      29.86       40.0       58.88 
Sp.gr.          1.297       1.423       1.728 

(Long,  W.  Ann.  1880,  11.  38.) 


ZINC  HYDRAZINE  CHLORIDE 


1121 


Sp.  gr.  of  ZnCl2+Aq  at  room  temp,  con- 
taining: 

15 . 334       23 . 487       33 . 752%  ZnCl2. 
1.1459        1.2288       1.3431 
(Wagner,  W.  Ann.  1883,  18.  267.) 

/       Sp.gr.  ofZnCl2+Aqat25°. 


Concentration  of  ZnCh 

+Aq 

Sp.  gr. 

1  —  normal 

V*—     " 

'/4—           " 

Vs—        " 

1.0590 
1.0302 
1.0152 
1  .  0077 

(Wagner,  Z.  phys.  Ch.  1890,  5.  40.) 
Sp.  gr.  of  ZnCl2+Aq. 


Yi  ZnCh  g.  in  1000  g. 
of  solution 

Sp.  gr.  16°/16° 

0 

1.000000 

0.5994 

1.000560 

2.3163 

1.002163 

5.0406 

1.004708 

9.8988 

1.009243 

19.4914 

1.018228 

(Dijken,  Z.  phys.  Ch.  1897,  24.  108.) 

Insol.   in   SbCl3.     (Klemensiewicz,    C.    C. 

1908,  II.  1850.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  830.) 

Easily  sol.  in  hot  absolute  alcohol,  and 
ether.  Sol.  in  1  pt.  strong  alcohol  at  12.5°. 
(Wenzel.) 

Sol.  in  0.35  pt.  absolute  alcohol.    (Graham .) 

Sol.  in  butyl  (Wurtz),  and  hexyl  (Bouis) 
alcohol  at  ord.  temp.,  but  decomp.  on  heating. 

Very  sol.  in  acetic  ether  with  evolution  of 
heat.  (Cann,  C.  R.  102.  363.) 

Easily  sol.  in  acetone.  (Krug  and  M'El- 
roy,  J.  Anal.  Ch.  6.  184.) 

1  g.  ZnCl2  is  sol.  in  2.3  g.  acetone  at  18°. 
Sp.  gr.  of  sat.  solution  18°/4°  =  1.14.  (Nau- 
mann,  B.  1904,  37.  4338.) 

Sol.  in  acetone  and  in  methylal.  (Eidmann, 
C.  C.  1899,  II.  1014.) 

Sol.    in   methyl   acetate.      (Naumann,    B. 

1909,  42.  3790.) 

Sol.  in  hot  benzonitrile,  also  in  other  aro- 
matic nitriles. 

Sol.  in  methyl  sulphide  and  in  ethyl  sul- 
phide. Very  sol.  in  piperidine.  (Werner,  Z. 
anorg.  1897,  16.  7.) 

Sol.  in  benzyl  alcohol,  furfurol,  methyl- 
propylketone,  acetophenone,  ethyl  mono- 
chloracetate,  ethyl  cyanacetate,  ethyl  aceto- 
acetate,  ethyl  benzoate,  ethyl  oxalate,  amyl 
nitrite,  pyridine,  piperidine,  and  quinoline. 

Insol.  in  salicylic  aldehyde,  ethyl  nitrate, 
and  nitrobenzene.  (Lincoln,  J.  phys.  Chem. 
1899,  3.  460.) 

Sol.  in  quinoline.  (Beckmann  and  Gabel, 
Z.  anorg.  1906,  51.  236.) 


Sol.  in  2  pts.  glycerine  at  ord.  temp. 
(Clever,  Bull.  Soc.  1872,  (2)  18.  372.) 

100  g.  glycerol  dissolve  50  g.  ZnCl2  at 
15.5°.  (Ossendowski,  Pharm.  J.  1907,  79. 
575.) 

Insol.  in  CS2.  (Arctowski,  Z.  anorg.  1894, 
6.  257.) 

Sol.  in  urethane.    (Castoro,  Z.  anorg.  1899, 

Mol.  weight  determined  in  piperidine; 
pyridine  and  methyl  sulphide.  (Werner,  Z. 
anorg.  1897,  16.  18.) 

+H2O.    Very  deliquescent.    Contains  11A 
H2O.    (Engel,  C.  R.  102.  1111.) 
Solubility  in  H2O. 
100  g.  of  the  sat.  solution  contain  at: 

0°  11°  27°  (mpt.) 

74.33         78.25        84.61  g.  ZnCl2. 

(Dietz,  Z.  anorg.  1899,  20.  245.) 


. 

Solubility  in  H2O. 
100  g.  of  the  sat.  solution  contain  at: 
0°          10°         20°         26°  (mpt.) 
67.45     73.65     80.08     83.43  g.  ZnCl2. 
(Dietz,  Z.  anorg.  1899,  20.  245.) 

+2H2O.     Sat.  aq.  solution  contains  at: 
—20°      —14°      —10°      —4°      —1° 
54.7       55.4       56.5       57.4      57.9%  salt, 

+5°          9°  15°          33°        42° 

59.1        60.2       62.0       66.8      68.  3%  salt. 
(Etard,  A.  ch.  1894,  (7)  2.  536.) 

Solubility  in  H2O. 

100  g.  of  the  sat.  solution  contain  at: 

0°      10°     19°  (mpt.) 

67  .56    73  .  70    79  .  07  g.  ZnCl2. 

(Dietz,  Z.  anorg.  1899,  20.  245.) 


.    Solubility  in  H2O  . 
lOd  g.  of  the  sat.  solution  contain  at: 

0°  8°  13°  (mpt.) 

67.42         71.96        75.  14  g.  ZnCl2. 

(Dietz,  Z.  anorg.  1899,  20.  245.) 

+3H2O.     Sol.  in   12.5  pts.     H2O  at  0°. 
(Engel.) 

Solubility  in  H2O. 
100  g.  of  the  sat.  solution  contain  at: 
—5°  0°  +7°  (mpt.) 

64.5          67.58        71  .  57  g.  ZnCl2. 
(Dietz,  Z.  anorg.  1899,  20.  245.) 

Zinc  hydrogen  chloride,  2ZnCl2,  HC1+2H20. 
Deliquescent.  (Engel,  C.  R.  102.  1068.) 
ZnCl2,  HC1+2H2O.  (Engel.) 

Zinc  hydrazine  chloride,  ZnCl2,  N2H4,  HC1. 

Very  hydroscopic. 

Sol.  in  H2O.     (Curtius,  J.  pr.  1894,  (2)  60. 
338.) 


1122 


ZINC  CHLORIDE  AMMONIA 


ZnCl-2.  2(N2H,,  HC1.)  Hydroscopic;  very 
sol.  in  H2O. 

Sol.  in  hot  alcohol  and  NH4OH+Aq.  (Cur- 
tius,  J.  pr.  1894,  (2)  50.  338.) 


Zinc  chloride  ammonia,  ZnCl2,  5NH3+H20. 

Easily  sol.  in  little,  but  decomp.  by  much 
H2O.  Still  more  sol.' in  ZnCl2+Aq  with  de- 
comp. (Divers,  C.  N.  18.  13.) 

ZnCl2>  4NH3+H2O.     (Kane.) 

ZnCl2,  2NH3.  Not  completely  sol.  in  H2O 
can  be  recryst.  from  hot  NH4Cl+Aq.  (Ritt- 
hausen,  J.  pr.  60.  473.) 

Insol.inH2O.  Sol.  in  NH4C1  or  NH4OH+ 
Aq.  (Thomas,  B.  20.  743.) 

+VAO. 

+2/6H20. 
+V2H20. 
+H20. 

(Andre",  C.  R.  1882,  94.  964.) 


Decomp.  by  H2O. 


ZnCl2,  NH3. 
ch.  72.  290.) 


Decomp.  by  H2O. 


(Kane,  A*. 


Zinc  chloride  cupric  oxide,  ZnCl2,  3CuO  + 

4H2O. 
(Mailhe,  C.  R.  1901,.  134.  226.) 

Zinc  chloride  hydrazine,  ZnCl2,  2N2H4. 

Ppt.     (Franzen,  Z.  anorg.  1908.  60.  275.) 

ZnCl2,  2N2H4.    Insol.  in  H2O. 

Easily  sol.  in  NH4OH-f  Aq.  (Curtius,  J. 
pr.  1894,  (2)  60.  345.) 

Zinc  chloride  hydroxylamine,  ZnCl2, 2NH2OH. 

SI.  sol.  in  cold,  somewhat  more  in  warm 
H2O.  Very  sol.  in  NH2OH+Aq.  Very  si. 
sol.  in  alcohol  and  other  organic  solvents. 
(Crismer,  Bull.  Soc.  (3)  3.  116.) 

1  pt.  is  dissolved  in  100  pts  aq.  solution 
sat.  at  20°.  (Antonoff,  C.  C.  1906,,  II.  810.) 

Zinc  fluoride,  ZnF2. 

SI.  sol.  in  cold,  more  easily  in  ho,t  H2O. 
Insol.  in  95%  alcdhpl.  Sol.  in  boiling  HNO3, 
HC1,  or  H2S04.  (Poulenc,  C.  R.  116.  581.) 

Contrary  to  older  statements,  ZnF2  is  quite 
sol.  in  H2O.  CKohlrausch,  Z.  phvs.  Ch.  1903, 
44.  213.) 

Insol.  in  liquid  NH3.  (Gore,  Amy  Ch  J 
1898,  20.  830.) 

Insol.  in  methyl  acetate.  (Naumann.  B. 
1909,  42.  3790.) 

+4H2O.  Difficultly  sol.  in  H2O.  Some- 
what more  sol.  in  H2O  containing  HF,  HC1, 
or  HNO3.  Easily  sol.  in  NH4OH+Aq. 
(Berzelius,  Pogg.  1.  26.) 

1  1.  H2O  dissolves  16  g.  at  18°.     (Dietz) 

Zinc  hydrogen  fluoride. 

Known  only  in  solution. 


Zinc  zirconium  fluoride. 
See  Fluozirconate,  zinc. 


Zinc  hydrophosphide,  Zn2H2P2. 

Decomp.  by  cold  H2O  and  by  dil.  HCl+Aq. 
(Drechsel  and  Finkelstein,  B.  1871,  4.  353.) 


Zinc  hydroxide,  Zn02H2. 

Insol.  in  H2O.  Sol.  in  acids.  Sol.  in  KOH. 
NaOH,  NH4OH,  or  (NH4)2CO3+Aq. 

1  1.  H2O  dissolve  0.01  g.  ZnO2H2  at  25°. 
(Bodlander,  Z.  phys.  Ch.  1898,  27.  66.) 

Solubility  in  H2O  is  calculated  to  be  2.6  X 
10:,5  g.  mols.  per  1.  (Herz,  Z.  anorg.  1900,  23. 
227.) 

1 1.  H2O  dissolves  0.0042  g.  ZnO2H2  at  18°. 
(Dupre  and  Bialas,  Z.  angew.  Ch.  1903,  16. 
55.) 

See  also  Zinc  oxide. 


Solubility  in  NH4OH+Aq  at  25°. 


ZnO2H2  used 

NHs  norm. 

G.  ZnO  per  1. 

prepared  from 

1.287 

7.28 

ZnSO4 

0.825 

3.84 

0.311 

0.85 

prepared  from 

Zn(N03)2 

0.321 
0.643 

0.34 
0.845 

1.215 

2.70 

1.928 

5.07 

2.570 

7.01 

3.213 

10.16 

(Bonsdorff,  Z.  anorg.  1904,  41.  189.) 

Solubility  of  ZnO2H2  in  NH4OH  and  am- 
monium bases +Aq  at  17°-19°. 


Normality  of  the  base 

G.  ZnO  in  20  cc.  of  the 
solution 

0.0942NH3 

0.00185 

0.236  NH3 

0.01795 

0.707NH3 

0.0959 

0.0944NH2CH3 

0.0008 

0.472NH2CH3 

0.01325 

0.944NH2CH3 

0.0484 

0.068NH2C2H5 

0.0005 

0.51NH2C2H5 

0.0074 

0.68NH2C2H5 

0.01605 

NH(C2H5)2 

insol. 

NH(CH3)2 

a 

(Herz,  Z.  anorg.  1902,  30.  280.) 


Solubility  in  NH4OH+Aq  increases  with 
ncreasing  concentration  of  NH4OH.  (Euler, 
B.  1903,  36.  3401.) 

2  pts.  ZnO2H2  dissolve  in  5  pts.  KOH+Aq. 
sp.gr.  =  1.3.)  (Bonnet.) 


ZINC  IODIDE 


1123 


Solubility  of  ZnO2H2  in  NaOH+Aq. 

Zinc  iodide,  ZnI2. 
Deliquescent.    Easily  sol.  in  H2O. 
Sat.  ZnI2-f  Aq  contains  at: 
—18°  —5°    +17°   47°     62°       73° 
70.9     74.0   80.4     80.3  81.3  81.2%ZnI2, 

97°      100°      107°      138°    140° 
82.1     83.0    82.6      83.8%  ZnI2. 
(Etard,  A.  ch.  1894,  (7)  2.  544.) 

Solubility  in  H2O. 

G.  Na  in  20  ccm. 

G.  Zn  in  20  ccm. 

0.1012 
0.1978 
0.4278 
0.6670 
0.9660 
1.4951 
2.9901 

0.0040 

0.0150 
0.0442 
0.1771 
0.9630 
0.2481 
0.3700 

When  zinc  hydroxide  is  treated  with 
alkali,  more  dissolves  .at  first  than  corre- 
sponds with  the  true  equilibrium  under  the 
prevailing  conditions,  for  such  solutions 
spontaneously  deposit  more  or  less  zinc 
hydroxide  according  to  the  concentration. 
(Rubenbauer,  Z.  anorg.  1902,  30.  333.) 

Solubility  of  ZnO2H2  in  NaOH+Aq  at  25C 


G.  mol.  per  1. 

1.234 

Sp. 
5 
1.045 

30 
1  .  368 

Na 

Zn 

0.2636 
0.3871 
0.5414 

0.9280 

0.00311 
0.0057 
0.0129 
0.0425 

(Wood,  Chem.  Soc.  1910,  97.  884.) 

Freshly  pptd.  ZnO2H2  is  easily  sol.  in 
KOH+Aq,  but  it  gradually  goes  over  into  a 
stable  form  which  is  difficultly  sol.  in  KOH+ 
Aq.  (Herz,  Z.  anorg.  1901,  28.  474.) 

Freshly  pptd.  ZnO2H2  is  sol.  in  dil.  salt 
solutions  (1  %)  as  follows.  The  given  amts. 
in  mg.  (calculated  as  Zn)  were  disolved  per 
1.  at  t°. 


Salt 

Mg.  Zn 

t° 

NaCl 
KC1   
CaCl2      
MgCl2     
BaCl2      .   •  
KoSO* 

51 
43 
57.5 
65 
38 
37.5 

18 
20 
16 
16 
18 
20 

MgSO4    
KNO3      

NaNO3 

27 
17.5 
22 

21 
15 
15 

Ba(NO3)2      
K2CO3     
NH4C1     
NH4NO3 

25 
0 
95 

77 

21 
15 
20 
20 

(NH4)2SO4 

88 

20 

(Snyders,  B.  11.  936.) 

+H20. 

See  also  Zinc  oxide. 

Zinc  hydrosulphide,  Zn(SH)2. 

Very  unstable.    Decomp.  by  H2O.    (Zotta, 
M.  10.  807.) 


Sol.    in    NaSH+Aq. 
2044.) 

Zn3H2S4.     (Zotta.) 


(Thomsen,    B.    11. 


100  g.  of  the  sat.  solution  contain  at: 
0°       18°      40°      60°      80°    100° 
81.11  81.20  81.66  82.37  83.05  83.62  g.  Znl,. 

(Dietz,  Z.  anorg.  1899,  20.  251.) 
See  also  under  +2H2O. 
Sp.  gr.  of  ZnI2+Aq  at  19.5°  containing: 
23.1       42.6       56.3       63.5     76.0%ZnI2. 
1.2340  1.5121    1.7871  1.9746  2.3976 

(Kremers,  Pogg.  111.  61.) 
Sp.  gr.  of  ZnI2+Aq  at  19.5°  containing: 

10          15          20          25     %ZnI2, 
1.045     1.091     1.140    1.196    1.255 


35 

1.390 


40 
1.420 


45 
1.560 


50     %ZnI2, 
1.650 


75 

2.360 


ZnI2. 


55          60          65          70 
1.754     1.8?5    2.020    2.180 

(Rremers,  calculated  by  Gerlach,  Z.  anal. 
8.  285.) 

Sol.  in  (NH4)2CO3-f  Aq. 

Moderately  sol.  in  liquid  NH3.  (Franklin, 
Am.  Ch.  J.  1898,  20.  830.) 

Sol.  in  alcohol. 

100  pts.  glycerine  disolve  40  pts.  at  ord. 
temp.  (Klever,  Bull.  Soc.  1872,  (2)  18.  372.) 

100  g.  glycerol  dissolve  40  g.  ZnI2  at  15.5°. 
(Ossendowski,  Pharm.  J.  1907,  79.  575.) 

More  sol.  in  anhydrous  ether  than  in  abs. 
alcohol.  Insol.  in  CS2.  (Hampe,  Ch.  Z. 
1887,  11.  846.) 

Sol.  in  methyl  acetate  (Naumann,  B. 
1909,  42.  3790);  acetone.  (Eidmann,  C.  C. 
1899,  II.  1014;  Naumann,  B.  1904,  37. 
4328.) 

Sol.  in  quinoline.  (Beckmann  and  Gabel, 
Z.  anorg.  1906,  61.  236.) 

Mol.  weight  determined  in  methyl  sul- 
phate. (Werner,  Z.  anorg.  1897,  15.  25.) 

+2H2O.    Solubility  in  H2O. 

100  g.  of  the  sat.  solution  contain  at: 
__!0°  —5°      0°      +10°      22°      27°(mpt.) 
80.50  80.77  81.16  82.06  83.12  89.52  g.  ZnI2. 
(Dietz,  Z.  anorg.  1899,  20.  251  .) 

+4H2O.     (Lubarski,  Z.  anorg.   1898,  18. 

387.) 


,  Znl4. 

Known  only  in  aqueous  solution.     (Baup, 
Repert.  14.  412.) 

Sol.   in   fenchone.      (Rimini   and   Olivari, 
C.  1907,  II.  241.) 


1124 


ZINC  IODIDE  AMMONIA 


Zinc  iodide  ammonia,  ZnI2,  4NH3. 

Decomp.  by  cold  H2O.  Easily  sol.  in  acids 
and  NH4OH+Aq.  (Rammelsberg,  Pogg. 

ZnI2,'5NH3.  Decomp.  by  cold  H2O.  Sol. 
in  NH4OH+Aq.  (Rammelsberg.) 

3ZnI2.  5NH3+3H2O.  (Tassily,  C.  R.  1896, 
122.  324.) 

Zinc  iodide  hydrazine,  ZnI2,  2N2H4. 

Decomp.  by  H2O. 

Sol.  in  NH4OH+Aq.  (Franzen,  Z.  anorg. 
1908,  60.  277.) 

Zinc  nitride,  Zn8N2. 

Decomp.  by  H2O  with  the  greatest  violence. 
(Frankland,  Phil.  Mag.  (4)  16.  149.) 

Easily  decomp.  by  H2O  when  finely  pow- 
dered. (Rossel,  C.  R.  1895,  121.  942.) 

Sol.  in  HC1.     (Fischer,  B.  1910,  43.  1468.) 

Zinc  oxide,  ZnO. 

Insol.  in  H2O.  Some  preparations  of  ZnO 
are  si.  sol.  in  H2O,  never,  however,  in  less 
than  1  million  pts.  H2O.  (Bineau,  C.  R.  41. 
510.) 

Calculated  from  electrical  conductivity 
of  ZnO+Aq.  1  pt.  ZnO  is  sol.  in  236,000 
pts.  H2O  at  18°.  (Dupre  and  Bialas,  Zeit. 
angew.  Ch.  1903,  16.  55.) 

See  also  Zinc  hydroxide. 

Easily  sol.  in  acids,  even  after  ignition. 
Easily  sol.  in  acids,  even  H2SO3,  or  H2CO3+ 
Aq. 

Solubility  of  ZnO  in  CrO3+Aq  at  25°. 
1  1.  of  the  solution  contains: 


G.CrOs 


0.010 

0.010 

0.010 

0.604 

2.14 

4.19 

11.4 

11.5 

22.2 

31.4 

43.1 

57.5 

66.5 

66.7 

70.6 

93.3 


G.  ZnO 


0.013 

0.013 

0.013 

0.409 

1.16 

2.24 

5.84 

5.89 

10.7 

14.9 

20.1 

26.7 

30.3 

30.4 

32.2 

41.5 


G.  CrO3 


101 

151 

192 
192 
285 
392 
450 
461 
463 
475 
574 
660 
769 
879 
970 


G.ZnO 


44.9 
66.1 
83.8 
83.6 

123 

168 

193 

196 

197 

202 

240 

274 

318 

354 

389 


(Groger,  Z.  anorg.  1911,  70.  136.) 

When  moist  is  easily  sol.  in  KOH,  NaOH, 
and  NH4OH+Aq.  but  only  si.  sol.  therein 
after  ignition.  Partially  repptd.  from  solu- 
tion in  NH4OH+Aq  by  dilution  with  H2O. 

Anhydrous  ZnO  is  insol.  in  dil.,  but  sol 
in  cone,  alkali  hydrates +Aq,  but  the  hy- 
droxide is  easily  sol.,  even  in  dil.  alkalies +Aq 
(Fremy,  A.  ch.  (3)  23.  390.) 

Very  si.  sol.  in  NH4OH+Aq.    After  igni- 


ton its  solubility  is  greatly  increased  by 
:races  of  K  and  NH4  salts.  Phosphates  have 
strongest  action,  then,  in  the  following 
order:  arsenates,  chlorides,  sulphites,  ni- 
brates,  acetates,  carbonates,  tartrates,  cit- 
rates, and  sulphates.  Succinates  and  ben- 
zoates  increase  the  solubility  in  NH4OH  + 
Aq,  only  when  it  is  very  dil.;  borates,  iodides, 
chlorates,  arsenites,  gallates,  and  oxalates 
do  not  increase  the  solubility.  (Schindler.) 

ZnO  is  sol.  in  NH4OH+Aq.  only  in  pres- 
nce  of  NH4  salts.  (Brandhorst,  Zeit.  an- 
gew. Ch.  1904,  17.  513.) 

Solubility  in  KOH,  NaOH,  and  NH4OH  + 
Aq. 

An  excess  over  4  mols.  KOH  to  1  mol. 
ZnO  is  necessary  for  solution,  but  that  excess 
may  be  neutralised  after  solution,  until  only 
4  mols.  are  left,  without  pptn.  of  ZnO.  Solu- 
tion is  pptd.  by  addition  of  12  vols.  H2O. 
KOH+Aq  containing  16.5  g.  KOH  to  a  litre 
H20  is  the  weakest  solution  which  will  dis- 
solve ZnO.  Three  times  as  much  alkali  are 
necessary  for  solution  at  50°  as  at  16-17°. 
Less  excess  of  NaOH  than  of  KOH  is  neces- 
sary. 3  mols.  NH4OH  will  dissolve  1  mol. 
ZnO,  and  the  temp,  and  dilution  are  in  this 
case  of  little  influence.  (Prescott.) 

100  cc.  of  20%  NaOH+Aq  dissolve  in 
many  hours  at  most  2.97  g.  ignited  ZnO. 
Pptd.  ZnO  is  more  quickly  dissolved  but  the 
action  becomes  very  slow  after  100  cc.  of  the 
solution  contain  3.87  g.  of  Zn.  (Forster  and 
Giinther,  Z.  Elektrochem.  1900,  6.  301.) 

Solubility  of  ignited  ZnO  in  NaOH+Aq 
gradually  decreases,  (Kunschert,  Z.  anorg. 
1904,  41.  343.) 

Sol.  in  hot  NH4Cl+Aq,  either  when  moist 
[>r  dry. 

Somewhat  less  sol.  in  NH4NO3+Aq. 

Somewhat  sol.  in  water  glass -f  Aq.  (Ord- 
way.) 

Slowly  sol.  in  cold,  easily  in  hot  NaCl+Aq. 
(Siersch,  J.  B.  1867.  255.) 

Solubility  of  ZnO  in  ZnCl2+Aq  at  room  temp. 


.  ZnCl2  per  100  g.  H2O         G.  ZnO  per  100  g.  H2O 


8.22 

23.24 

45.95 

51.50 

56.90 

62.85 

96.00 

124.70 

144.80 

203.00 


0.0137 

0.138 

0.497 

0.604 

0.723 

0.884 

1.792 

3.213 

2.640 

1.590 


The  solubility  curve  has  a  maximum  at  a 
point  corresponding  to  about  125  g.  ZnCl2  per 
100  g.  H2O.  On  the  first  branch  of  the  curve 
the  solid  phase  in  equilibrium  with  the  solu- 
tion is  ZnCl2,  4ZnO,  6H2O;  on  the  second 
branch  it  is  ZnCl2,  ZnO,  1.5H2O. 

(Driot,  C.  R.  1910,  160.  1427.) 


ZINC  PHOSPHIDE 


1125 


Sol.  in  boiling  Fe(NO3)3,  and  Pb(NO3)2  + 
Aq  with  pptn.  of  oxides.  Not  attacked  by 
Co(N03)2,  Ni(NO,),,  and  Ce(NO,),+Aq. 
(Persoz.) 

Sol.  in  boiling  KCN+Aq. 

Insol.  in  boiling  K  tartrate  +Aq.  (Kah- 
lenberg  and  Hillyer,  Am.  Ch.  J.  1894,  16.  101.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  830.) 

Tartar ic  acid  somewhat  hinders  the  pptn. 
of  ZnO2H2. 

Insol.  in  methyl  acetate.  (Naumann,  B. 
1909,  42.  3790.) 

Insol.  in  acetone.  (Naumann,  B.  1904, 
37.  4329;  Eidmann,  C.  C.  1899,  II.  1014.) 

Sol.  in  methyl  amine,  but  insol.  in  amyl 
amine+Aq.  (Wurtz.) 

1  1.  solution  containing  174.4  g.  sugar 
and  14.1  g.  CaO  dissoolves  0.24  g.  ZnO. 
(Bodenberider,  J.  B.  1865,  600.) 

Min.  Zincite.    Sol.  in  acids. 

Zinc  peroxide. 

1  pt.  sol.  in  45,000  pts.  H2O. 

Very  sol.  in  acids.  (Foregger  and  Philipp, 
J.  Soc.  Chem.  Ind.  1906,  25.  300.) 

Zn02  (?).  Ppt.  Decomp.  by  acids  with 
evolution  of  H2O2.  (Haass,  B.  17.  2249.) 

ZnO,  H2O,  H2O2.  (de  Forcrand,  A.  ch. 
1902,  (7)  27.  58.) 

3ZnO,  2H2O2.     (de  Forcrand.) 

3ZnO,  H2O,  2H2O2.     (de  Forcrand.) 

4ZnO,  H2O,  3H2O2.     (de  Forcrand.) 

ZnO2,  ZnO2H2.  Insol.  in  NH4OH+Aq 
(Kouriloff,  A.  ch.  (6)  23.  431.) 

3Zn02,  Zn(OH)2.  Sol.  in  NaOH  +Aq  with 
evolution  of  O.  (Eijkman,  C.  C.  1906,  I. 
1628.) 

Zii4O7,  3ZnO+4H2O.  Completely  sol.  in 
dil.  H2SO4.  (de  Forcrand.) 

10ZnO2,  4ZnO+5H2O.  Ppt.  (Teletow 
C.  C.  1911,  I.  1799.) 

Zinc  oxybromide,  ZnBr2,  ZnO+13H2O. 

ZnBr2,  4ZnO  +  10,  13,  and  19H2O.  De- 
comp. by  H2O  into — 

ZnBr2,  6ZnO+35H2O.     (Andre".) 
ZnBr2,  5ZnO+6H2O.     (Andre*.) 
All    oxybromides    are    sol.    in    KOH    anc 
NH4OH+Aq.     (Andr6,  C.  R.  96.  703.) 

Zinc   oxybromide   ammonia,   ZnBr2,    3ZnO 

2NH3+5H2O. 
Decomp.  by  H2O.    (Andre*,  C.  R.  96.  703. 

Zinc  oxychloride,  ZnO,  3ZnCl2+H2O. 

Decomp.  by  H2O. 

Very  sol.  in  dil.  acids.  (Ephraim,  Z.  anorg 
1908,  59.  67.) 

+4H2O.  SI.  sol.  in  H2O;  more  sol.  IE 
ZnCl2+Aq. 

Easily  sol.  in  acids,  or  NH4OH,  or  KOH  + 
Aq.  (Schindler,  Mag.  Pharm.  36.  45.) 

+5H2O  and  8H2O.  (Andre",  A.  ch.  (6)  3 
94.) 


ZnO,  ZnCl2  +  lMH2O.  (Driot,  C.  R.  1910, 
50.  1427.) 

3ZnO,  ZnCl2+2H2O.  SI.  sol.  in  H2O, 
nore  easily  sol.  in  ZnCl2+Aq.  Easily  sol. 
n  acids  and  in  NH4OH  or  KOH+Aq. 
Schindler,  Mag.  Pharm.  36.  45.) 

+3H2O.      (Werner,    B.    1907,   40.   4443.) 

+5H2O.    (Mailhe,  A.  ch.  1902,  (7)  27.  367.) 

3ZnO,  2ZnCl2+llH2O.  (Andre*,  C.  R. 
888,  106.  854.) 

4ZnO,  ZnCl2+6H2O.  (Andre*,  C.  R.  1888, 
106.  854.) 

+  11H2O.    (Andre,  A.  ch.  (6)  3.  94.) 

5ZnO,  ZnCl2+6H2O.  (Perrot,  Bull.  Soc. 
1895,  (3)  13.  976.) 

+8H2O.     (Andre",  C.  R.  1882,  94.  1524.) 

5ZnO,  2ZnCl2+26H2O.  Sol.  in  KOH  or 
NH4OH+Aq.  Decomp.  by  H2O  into — 

5ZnO,  ZnCl2+26H2O.  Sol.  in  KOH  or 
NH4OH+Aq.  Decomp.  by  H2O  into— 

6ZnO,  ZnCl2+6H2O.  Insol.  in  H2O. 
:Kane,  A.  ch.  72.  296.) 

8ZnO,  ZnCl2  +  10H2Q.  (Mailhe,  A.  ch. 
1902,  (7)  27.  367.) 

9ZnO,  ZnCl2+3H2O.  Insol.  in  H2O. 
Less  sol.  in  NH4OH+Aq  than  ZnCl2,  3ZnO  + 
2H2O,  but  easily  sol.  in  +14H2O. 

9ZnO,  2ZnCl2  +  12H2O.  Insol.  in  hot  or 
cold  H2O.  (Habermann,  M.  6.  432.) 

Zinc    oxychloride    ammonia,    6ZnCl2,    ZnO, 

12NH3+4H2O. 
Decomp.    by    H2O    and    boiling    alcohol. 

(Andre",  A.  ch.  (6)  3.  90.) 
ZnCl2,     3ZnO,     2NH3+5H2O.      Decomp. 

by  H2O.     (Andre*.) 

ZnCl2,  2ZnO,  2NH3+3H2O.  (Andre".) 
6ZnCl2,  3ZnO,  10NH3  +  13H2O.  (Andre.) 
4ZnCl2,  ZnO,  8NH3+2H2O.  -  (Andre.) 

Zinc  oxyiodide,  ZnI2,  3ZnO+2H2O. 

Insol.  in  cold,  si.  sol.  in  boiling  H2O. 
(Muller,  J.  pr.  26.  441.) 

ZnI2,  9ZnO+24H2O.    Insol.  in  cold  H2O. 

ZnI2,  5ZnO  +  llH2O.  Decomp.  by  H2O. 
(Tassilly,  C.  R.  1896,  122.  324.) 

Zinc  oxyphosphide,  ZnP2O. 

(Renault,  A.  ch.  (4)  9.  162.) 

Probably  is  a  mixture  of  zinc  phosphate 
and  phosphorus.  (Vigier,  Bull.  Soc.  1861. 
5.) 

Zinc  oxysulphide,  ZnO,  ZnS. 

Sol.  in  HCl+Aq.    (Arfvedson,  Pogg.  1.  59.) 
4ZnS,    ZnO.      Not    decomp.    by    boiling 
HC2H3O2+Aq.    (Kersten,  Schw.  J.  57.  186.) 
Min.  Volzite.    Sol.  in  HCl+Aq. 

Zinc  phosphide,  ZnP. 

Less  easily   attacked  by   HCl+Aq  than 

ZnP2.     Not   attacked   by   hot   HCl+Aq. 
(Hvoslef,  A.  100.  99.) 
ZnP4.    Insol.  in  dil.  HCl+Aq.     (Renault.) 


1126 


ZINC  SELENIDE 


Zn3P2.  Insol.  in  H2O.  Sol.  in  dil.  HC1, 
H2SO4,  or  HNO3+Aq,  with  evolution  of 
PH3.  (Renault,  A.  ch.  (4)  9.  162.) 

Zn3P4.      Insol.   in   HCl+Aq.      (Renault.) 

Zinc  selenide,  ZnSe. 

Cold  dil.  HNO3+Aq  dissolves  out  Zn,  and 
Se  separates  out,  which  dissolves  on  warming 
as  H2SeO3.  (Berzelius.) 

+zH20.    Insol.  in  H2O.     (Berzelius.) 

Zinc  sulphide,  ZnS. 

Anhydrous.  Insol.  in  H2O.  Sol.  in  HC1+ 
Aq;  insol.  in  HC2H3O2+Aq.  (Ebelmen,  A. 
ch.  (3)  26.  97.) 

Sol.  in  H2S+Aq  under  pressure  in  a  sealed 
tube.  (Senarmont,  A.  ch.  (3)  32.  168.) 

Min.  Blende,  Sphalerite.  SI.  attacked  by 
acids,  expecting  aqua  regia. 

1  1.  H2O  dissolves  6.65  X10-6  mols.  zinc 
blende  at  18°. 

1  1.  H2O  dissolves  6.63  Xlp-6  mols.  arti- 
ficial cryst.  ZnS  at  18°.  (Wiegel,  Z.  phys. 
Ch.  1907,  68.  294.) 

Sol.  in  an  alkaline  solution  of  NaClO. 
(Sadtler,  Trans.  Am.  Electrochem.  Soc. 
1902,  1.  142.) 

Insol.  in  liquid  NH3.  (Franklin,  Am.  Ch. 
J.  1898,  20.  830.) 

+1/2,  2/3,  or  1H2O. 

Pptd.  ZnS. 

1  1.  H2O  dissolves  70.60  XKH5  mols.  pptd. 
ZnS  at  18°.  (Wiegel,  Z.  phys.  Ch.  1907,  58. 
294.) 

Insol.  in  alkali  hydrates,  carbonates,  and 
sulphides +Aq.  Insol.  in  NH4OH,  HC1,  or 
(NH4)2CO3+Aq.  Easily  sol.  in  very  'dil.  HC1 
and  HNO3+Aq,  but  H2S  ppts.  ZnS  in  pres- 
ence of  very  dil.  HCl+Aq,  or  H2S04+Aq. 
(Eliot  and  Storer.) 

More  easily  sol.  in  HNO3+Aq  than  in 
HCl+Aq.  (Fresenius.) 

Only  si.  sol.  in  acetic  acid.    (Wackenroder.) 

When  still  moist  is  sol.  in  H2S03+Aq. 

Insol.  in  NH4C1  or  NH4NO3+Aq. 

K2S+Aq  when  added  to  ZnS04+Aq  pro- 
duces a  ppt.  in  presence  of  fO,000  pts.  H2O, 
and  a  slight  opalescence  with  20,000  pts. 
(Lassaigne.) 

Slowly  sol.  in  cone.  KCN+Aq.  (Halm, 
J.  B.  1870.  1008.) 

SI.  sol.  in  Na2S+Aq;  sol.  in  NaSH+Aq. 
(Becker,  Sill.  Am.  J.  (3)  33.  199.) 

Zinc  peratasulphide,  ZnS5. 

Sol.  in  acids,  with  separation  of  S.  (Schiff, 
A.  116.  74.) 

Zinc  sulphosilicide,  ZnSiS. 

Decomp.  by  acids  and  by  alkalies.  (Fraen- 
kel,  Metall,  1909,  6.  683.) 

Zinc  telluride,  ZnTe. 

Decomp.  by  acids.  Sol.  in  Br2+Aq. 
(Fabre,  C.  R.  105.  277.) 


Zincic  acid. 

Zinc  hydroxide  shows  weak  acid  properties, 
and  forms  the  following  salts. 

Ammonium  zincate,  3ZnO,  4NH3+12H2O  = 

3ZnO,  2(NH4)2O+10H2O. 
Decomp.  by  much  H2O.  . 

Barium  zincate,  BaH2Zn2O4+7H2O. 

Decomp.  by  H2O.  (Bertrand,  C.  R.  116. 
939.) 

Calcium  zincate,  CaH2Zn2O4+4H2O. 

Decomp.  by  H2O.  Sol.  in  NH4OH+Aq. 
(Bertrand,  C.  R.  115.  939.) 

Cobaltous  zincate,  rcCoO,  ?/ZnO. 

Rinman's  green.  Sol.  in  acids.  H2CO3+Aq 
dissolves  out  ZnO.  (Comey.) 

Potassium  zincate,  ZnO,  K2O. 

Easily  sol.  in  H2O,  but  decomp.  by  boiling. 
(Laux,  A.  9.  183.) 

2ZnO,  K2O.  Decomp.  immediately  by 
cold  H2O.  (Fremy,  C.  R.  15.  1106.) 

Sodic  zincate,  Na2O,  2ZnO+8H2O,  or 
2NaHZnO2+7H2O. 

Decomp.  by  H2O  or  alcohol.  (Comey 
and  Jackson,  Am.  Ch.  J.  11.  145.) 

+7H2O.  (Forster  and  Gunther,  Z.  Elek- 
trochem,  1899,  6.  301.) 

2Na2O,  3ZnO  +  18H2O  or  Zn3O6Na4H2+ 
17H2O.  Decomp.  by  H2O  or  alcohol.  Insol. 
in  ether.  (Comey  and  Jackson.) 

Strontium  zincate,  SrH2Zn2O4+7H2O. 
Decomp.  by  H2O.     (Bertrand.) 

Zirconic  acid. 
See  Zirconium  hydroxide. 

Barium  zirconate,  BaZrO3. 

Insol.  in  acids.     (Ouvrard,  C.  R.  113.  80.) 

Calcium  zirconate,  CaZrO3. 

Insol.  in  acids.     (Ouvrard,  C.  R.  113.  80.) 

Calcium  zirconate,  acid. 

Inscl.  in  H2O  or  HCl+Aq.  (Hiordthal,  A. 
137.  237.) 

Calcium  potassium  zirconate,  (Ca,K)LaO3 
(small  quantity  of  CaO  substituted  by 
K20). 

Sol.  in  HC1.  (Venable,  J.  Am.  Chem.  Soc. 
1896,  18.  444.) 

Cupric  zirconate. 

(Berthier,  A.  ch.  59.  195.) 


ZIRCONIUM  IODIDE 


1127 


Lithium  zirconate,  Li2ZrO3. 

Easily  attacked  by  acids.  (Ouvrard,  C.  R 
112.  1444.) 

Magnesium  zirconate. 

Insol.  in  H2O  or  HCl+Aq.  (Hiordthal 
C.  R.  61.  215.) 

Potassium  zirconate. 

Decomp.  by  HCl+Aq.    (Knop,  A.  169.  44. 

Sodium  zirconate,  Na2ZrO3. 

Decomp.  by  H2O. 

Na4ZrO4.  Decomp.  by  HCl+Aq,  and  is 
dissolved  by  subsequent  addition  of  H2O 

Na2O,  8ZrO2  +  12H2O.     (Hiordthal.) 

Strontium  zirconate,  SrZrO3. 

As  CaZrO3.     (Ouvrard.) 

Zirconium,  Zr. 

Crystallized.  Attacked  by  cone.  HCl+Aq 
above  50°,  but  very  slowly  even  at  100° 
rapidly  by  hot  aqua  regia.  Sol.  in  cold  cone 
HF+Aq.  (Troost,  C.  R.  61.  109.) 

Very  violently  attacked  by  a  mixture  of 
HNO3  and  HF.  (Berzelius,  Pogg.  4.  117.) 

Amorphous.  Slowly  attacked  by  boiling 
aqua  regia,  H2SO4,  or  cone.  HCl+Aq.  (Ber- 
zelius.) 

Easily  sol.  in  HF  or  HNO3+HF. 

Zirconium  bromide,  ZrBr4. 

Very  hygroscopic.  Violently  decomp.  by 
H2O  to  form  oxybromide.  (Melliss,  Zeit. 
Ch.  (2)  6.  296.) 

SI.  sol.  in  organic  solvents.  (Matthews,  J. 
Am.  Chem.  Soc.  1898,  20.  840.) 

Zirconium  bromide  ammonia,  ZrBr4,  4NH3. 

Ppt.  Insol.  in  organic  solvents.  (Mat- 
thews, J.  Am.  Chem.  Soc.  1898,  20.  840.) 

ZrBr4,  10NH3.     Very  hydroscopic. 

Decomp.  by  H2O.  (Stabler,  B.  1905,  38. 
2612.) 

Zirconium  carbide,  ZrC. 

Insol.  in  H2O  and  NH4OH+Aq  and  HC1 
Aq  even  when  heated.  Sol.  in  HNO3,  HaSO4 
and  fused  alkali  nitrates,  chlorates,  or  hy- 
droxides. (Moissan,  C.  R.  1896,  122.  653.) 

Zirconium  chloride,  ZrCl4. 

Sol.  in  H2O  with  evolution  of  much  heat 
to  form  ZrOCl2.  Sol.  in  alcohol.  (Hinsberg, 
A.  239.  253.) 

Very  unstable. 

Probably  substances  so  described  in  the 
literature  by  Nylander  and  others  were  oxy- 
chlorides.  (Venable,  J.  Am.  Chem.  Soc.  1894, 
16.  471.) 

Sol.  in  ether.  (Matthews,  J.  Am.  Chem. 
Soc.  1898,20.821.) 


Zirconium  chloride  ammonia,  ZrCl4,  2NHL 
Fumes   in    the    air.      Decomp.    by   H2O. 

(Matthews,  J.  Am.  Chem.  Soc.  1898,  20.  821.) 
ZrCl4,  3NH3.  (Stabler,  B.  1905,  38.  2611.) 
ZrCl4,  4NH3.  Decomp.  by  H2O.  (Pay- 

kull.) 

Unstable.    Decomp.  by  H2O.    (Matthews, 

J.  Am.  Chem.  Soc.  1898,  20.  821.) 

ZrCl4,  8NH3.    Stable  in  the  air.    Decomp. 

by  H2O.     Insol.  in  ether.      (Matthews,   J. 

Am.  Chem.  Soc.  1898,  20.  821.) 

Very    hydroscopic.      Decomp.    by    H2O. 

(Stabler,  B.  1905,  38.  2611.) 

Zirconium  fluoride,  ZrF4. 

Anhydrous.  Insol.  in  H2O  and  acids.  (De- 
ville,  A.  ch.  (3)  49.  84.) 

Only  si.  sol.  in  H2O. 

1.388  g.  dissolve  in  100  cc.  H2O  without 
hydrolysis.  On  warming  the  solution,  zir- 
conium hydrate  begins  to  ppt.  out  at  about 
50°.  (Wolter,  Ch.  Z.  1908,  32.  606.) 

+3H2O.  Sol.  in  H2O,  but  solution  decom- 
poses on  diluting,  with  pptn.  of  an  insol. 
basic  salt.  Sol.  in  dil.  HF+Aq.  (Berzelius.) 

Zirconium  fluoride  ammonia,  5ZrF4,  2NH8. 
(Wolter,  Ch.  Z.  1908,  32.  607.) 

Zirconium  hydride,  ZrH2. 

Not  attacked  by  acids.     (Winkler,  B.  24.     < 

873.) 

Zirconium  hydroxide,  Zr(OH)4. 

Insol.  in  H2O  or  alcohol.  Sol.  in  5000  pts. 
H20.  (Melliss.) 

Sol.  in  acids,  even  oxalic  or  tartaric  acid, 
when  precipitated  cold.  If  precipitated  hot, 
t  is  slowly  dissolved  upon  heating  with  cone, 
acids. 

Sol.  in  dil.  or  cone.  min.  acids  except  HI. 
Readily  sol.  in  oxalic,  only  si.  sol.  in  acetic 
acid. 

Much  less  sol.  when  pptd.  from  hot  splu- 
ion  than  when  pptd.  from  cold  solution. 
Venable,  J.  Am.  Chem.  Soc.  1898,  20.  274.) 

SI.  sol.  in  (NH4)2CO3+Aq.  Insol.  in 
£2CO3  and  Na2CO3+Aq.  Insol.  in  NaOH, 
£OH,  and  NH4OH+Aq. 

Sol.  in  (NH4)2C4H4O6+NH4OH+Aq.  In- 
sol. in  NH4  salts +Aq. 

Zirconium  iodide,  ZrI4. 

Fumes  in  the  air. 

Sol.  in  H2O  and  acids  with  violent  re- 
.ction. 

Decomp.   by  alcohol.   Sol.  in  abs.   ether. 

SI.  sol.  in  benzene  and  CS2.  (Stabler,  B. 
904,  37.  1137.) 

Insol.  in  H2O,  HNO3,  HC1,  aqua  regia, 
,nd  CS2. 

Sol.  in  H2SO4  with  decomp;  unchanged 
>y  boiling  H2O.  (Dennis,  J.  Am.  Chem. 
*oc.  1896,  18.  678.) 


1128 


ZIRCONIUM  IODIDE  AMMONIA 


Zirconium    iodide    ammonia,    ZrI4,    6NH3; 

ZrI4,  7NH3;  ZrI4,  8NH3;  ZrI4,  10NH3. 
All  above  comps.  are  hydroscopic  and  lose 
NH3  in  the  air.    (Stabler,  B.  1905,  38.  2615.) 

Zirconium  nitride. 

Scarcely  attacked  by  acids,  aqua  regia,  and 
caustic  alkalies.  Slowly  -decomp.  by  long 
contact  with  H2O.  (Mallet,  Sill.  Am.  J.  (2) 
28.  346.) 

Zr2N3.  Decomp.  when  heated  in  the  air; 
sol.  in  HF;  insol.  in  other  min.  acids.  (Mat- 
thews, J.  Am.  Chem.  Soc.  1898,  20.  844.) 

ZrsNp.     Decomp.  when  heated  in  the  air. 

Sol.  in  HF;  insol.  in  other  min.  acids.  (Mat- 
thews, J.  Am.  Chem.  Soc.  1898,  20.  844.) 

Zirconium  oxide,  ZrO2. 

When  ignited,  is  insol.  in  all  acids  except 
HF  and  H2SO4.  SI.  sol.  in  HF;  sol.  in  H2SO4 
only  when  very  finely  powdered  and  heated 
with  a  mixture  of  2  pts.  H2SO4  and  1  pt.  H2O 
until  the  H2SO4  volatilises.  (Berzelius.) 

Zirconium  peroxide,  ZrO3. 

(Cleve,  Bull.  Soc.  (2)  43.  53),  or  Zr205  ac- 
cording to  Bailey  (Chem.  Soc.  49.  150). 

Not  attacked  by  cold  dil.  H2SO4+Aq. 
(Bailey.) 

Zirconium  silicon  oxide. 

Min.  Zircon.    See  Silicate,  zirconium. 

Zirconium  oxy-compounds. 
See  Zirconyl  compounds. 

Zirconium  phosphide,  ZrP2. 

Insol.  in  dil.  or  cone,  acids  and  alkalies. 
SI.  sol.  in  aqua  regia.     (Gewecke.  A.  1908. 
361.  85.) 

Zirconium  silicide,  ZrSi2. 

Sol.  in  HF,  insol.  in  other  min.  acids. 

Not  acted  upon  by  10%  KOH+Aq  or 
NaOH+Aq. 

Decomp.  by  fusion  with  KOH.  (Honigs- 
chmid,  C.  R.  1906,  143.  225.) 

Zirconium  sulphide. 

*  Insol.  in  H2O.  Sol.  in  HF;  slowly  sol.  in 
aqua  regia.  Insol.  in  HNO3,  HC1,  H2S04, 
or  KOH+Aq.  (Berzelius.) 

Insol.  in  dil.  acids.  Sol.  in  cone.  HN03+ 
Aq  (perhaps  an  oxysulphide) .  (Fremy.) 

Zirconomolybdic  acid. 

Ammonium  zirconomolybdate, 

2(NH4)2O,  ZrO2,  12MoO3+10H2O. 
Sol.  in  H2O.     (Pechard,  C.  R.  1893,  117. 
790.) 


Potassium  zirconomolybdate, 

2K2O,  ZrO2,  12MoO3  +  18H2O. 
Sol.  in  H2O.     (Pechard.) 

Zirconotungstic  acid. 

Ammonium  zirconoofecatungstate, 

3(NH4)2O,  ZrO2,  10WO3  +  13H2O. 

Very  sol.  in  H2O. 

Efflorescent.  (Hallopeau,  Bull.  Soc.  1896, 
(3)  15.  921.) 

3(NH4)2O,  H2O,  ZrO2,  10WO3+13H2O. 
Sol.  in  H20;  unstable;  effloresces  in  the  air. 
(Hallopeau.) 

Potassium  zirconotungstate,  4K2O.  ZrO2, 
WO3+20H2O. 

Sol.  in  hot  H2O.     (Hallopeau.) 

4K2O,  ZrO2,  10WO3+15H2O.  More  sol. 
in  hot  than  in  cold  H2O. 

Sol.  in  fused  alkali  carbonates.  (Hallo- 
peau.) 

Potassium  cKzirconocfecatungstate, 

4K2O,  2ZrO2,  10WO3+20H2O. 
More  sol.  in  hot  than  in  cold  H2O. 
Sol.  in  fused  alkali  carbonates.  (Hallopeau.) 

Zirconyl  bromide,  ZrOBr2+3H2O. 

Deliquescent.  Decomp.  in  moist  air. 
Very  sol.  in  H2O.  .(Venable,  J.  Am.  Chem. 
Soc.  1898,  20.  324.) 

+7H2O.     Sol.  in  H2O.     (Melliss.) 

+8H20.  Deliquescent.  Decomp.  in  moist 
air.  Very  sol.  in  H2O.  (Venable,  J.  Am. 
Chem.  Soc.  1898,  20.  324.) 

+  13H2O.  Deliquescent.  Decomp.  in 
moist  air. 

Very  sol.  in  H2O.    (Venable.) 

+  14H2O.  Deliquescent.  Decomp.  in 
moist  air.  (Venable.) 

Very  sol.  in  H2O.     (Venable.) 

ZrBr(OH)3+H2O,  and  +2H2O.  Deliques- 
cent, and  decomp.  in  moist  air.  (Venable.) 

Zirconyl  chloride,  ZrOCl2. 

Sol.  in  H2O;  insol.  in  HC1.  (Venable,  J. 
Am.  Chem.  Soc.  1894,  16.  475.) 

+2H2Q.  (Chauvenet,  C.  R.  1912,  164. 
822.) 

+3H2O.     Sol.  in  H2O.     (Venable.) 

d-3.5H2O.  (Chauvenet,  C.  R.  1912,  154. 
822.) 

+6H2O.     (Chauvenet.) 

Sol.  in  H2O. 

Insol.  in  HC1.     (Venable.) 

+4^H2O,  6^H2O,  and  8H2O. 

Efflorescent.  Easily  sol.  in  H2O  and  alco- 
hol. Very  si.  sol.  in  cone.  HCl+Aq.  (Ber- 
zelius.) 

+8H2O.  Sol.  in  H2O.  (Venable,  J.  Am. 
Chem.  Soc.  1898,  20.  321.) 

Effloresces  in  the  air. 


ZIRCONYL  SULPHIDE 


1129 


Sol.  in  H2O.  Less  sol.  in  HCl+Aq.  and 
nearly  insol.  in  cone.  HC1.  (Chauvenet, 
C.  R.  1912,  154.  822.) 

Zr2OCl2.  Sol.  in  H2O  and  alcohol.  (Ende- 
mann,  J.  pr.  (2)  11.  219.) 

Not  decomp.  by  H2O. 

Sol.  in  dil.  HC1.  (Chauvenet,  C.  R.  1912, 
154.  1236.) 

+H2O.  (Chauvenet,  C.  R.  1912,  154. 
1236.) 

-f  3H2O.  Decomp.  by  H2O.  Sol.  in  dil 
HC1.  (Chauvenet.) 

8ZrO2,  7HC1.    Sol.  in  H2O.    (E.) 

Zr2OCl6.  (Troost  and  Hautefeuille,  C.  R. 
73.  563.) 


Zr3OCl4=ZrCl4,  2ZrO2.  Insol.  in  H2O. 
(Hermann.) 

Zirconyl  iodide,  ZrOI2+8H2O. 

Very  sol.  in  H2O  and  alcohol. 

Very  hydroscopic.  ((Stabler,  B.  1904, 
37.  1138.) 

ZrI(OH)3+3H2O.  Easily  sol.  in  H2O. 
(Hinsberg,  A.  239.  253.) 

Ppt.  SI.  sol.  in  HI+Aq.  (Venable,  J. 
Am.  Chem.  Soc.  1898,  20.  328.) 

Zirconyl  sulphide  (?) 

Decomp.  by  HNO3  with  separation  of  S. 
(Fremy,  A.  ch.  (3)  38.  326.) 


APPENDIX 


FORMULAE  FOR  CONVERTING  AREOMETER  DEGREES  INTO 
,     SPECIFIC  GRAVITY. 

n  =no.  of  degrees  on  the  areometer  scale;  sp.  gr.  =  specific  gravity. 


Areometer 

Temp. 

Liquids  heavier  than  HaO 

Liquids  lighter  than  HzO 

1.  Baume. 

(a)    According   to   Baume'  s 
original       directions.          For 
Kquids    heavier    than    H2O. 
Sp.  gr.  of  a  solution  of  15  pts. 
NaCl  dissolved  in  85  pts  H2O 

15° 

SD          -    149'°5 

s               -    145'56 

(12  5°                      \ 
dj7^  =  1.1118988j 

=  15°;  H2O  =  0°.    For  liquids 
lighter  than  H2O.    Sp.  gr.  of 
10%     NaCl+A*q     at     12.5° 
/  12  5°                     \ 

fep<  gr>  "  149.05-n 

Sp>gr"   -135.56+n 

I    12  5°  ~                    I     "  i 
H2O  =  10°. 

145.88 

145.88 

(6)     Old     Form.       Liquids 
heavier  than  H2O,  10%NaCl 

-f  Aq-at  15°  (  4JL  =  1.073350') 

12.5 
1^° 

bp'gr-     145.  88  -n 
-    146'3 

bp-gr-     135.88+n 
146.3 

\  15                     1 
=  10°;      H2O  =  0°.        Liquids 
lighter  than  H2O,  10%  NaCl 

fep'gr-     146.  3-n 
146.78 

^•^•"136.3+71 
Sp  £r        146'78 

+Aq  —  0  ,M2O  —  10  . 
(c)  New    Form.      So-called 
"  Rational    Scale."      Liquids 
heavier  than  H2O,   H2SO4  + 
1  ^° 

17.5 

1  K° 

^•^'     146.  78  -n 
°p  er        144'3 

hp>gr'     136.78+n 

Aq-^j  =  1.842  =  66°;  H2O  =  0°. 

JLo 

15 

bp>gr'     144.  3  -n 

2.  Beck. 

H2O  =  0°;    liquid   of   0.850 

/I  o  eo\ 
1     -  ^O°         ^r>ala 

170 

Sn          -   17° 

°f-  &l'\  12  5°/                ocaie 
continued  above  and  below. 

12.5°  . 

Sp'gr-     170-n 

Sp.gr.  -170+n 

3.  Twaddle. 
H2O  =  0°.    Each  degree  cor- 
responds   to    an   increase    of 
0.005  in  the  sp.  gr. 

Given  on 
the  instru- 
ment 

Sp.gr.  =  1.000+0.005» 

1132 


APPENDIX 


TABLES  FOR  THE  CONVERSION  OF  BAUMfi  DEGREES 
INTO  SP.  GR. 

Since  the  original  directions  of  Baume  there  have  been  many  slight  modifica- 
tions suggested,  so  that  there  are  several  varieties  of  Baume  hydrometers  with 
somewhat  varying  readings,  tables  for  the  two  principal  ones  of  which  are  here- 
given. 

1.  According  to  Baume's  original  directions. 
For  liquids  heavier  than  H2O.    Sp.  gr.  of  15  %  NaCl+ 
Aq  (^ps)  =  1.1118988  =  15°;  H2O  =  0°. 

149.05 


Calculated  according  to  the  formula,  sp.  gr.  = 


149.05  -n. 


Deg. 

Baum6 

Sp.  gr. 

Deg. 
Baume 

Sp.  gr. 

Deg. 

Baum6 

Sp.  gr. 

Deg. 

Baum6 

Sp.  gr. 

0 

.00000 

20 

.  15497 

39 

1.35438 

58 

1.63701 

1 

.00675 

21 

.  16399 

40 

1.36680 

59 

1.65519 

2 

.01360 

22 

1.17316 

41 

1.37945 

60 

1.67378 

3 

.02054 

23 

.  18246 

.  42 

1.39234 

61 

1.69279 

4 

.02757 

24 

1.19192 

43 

1.40547 

62 

1.71223 

5 

.03471 

25 

1.20153 

44 

1.41885 

63 

1.73213 

6 

.04194 

26 

1.21129 

45 

1.43248 

64 

1.75250 

7 

.04927 

27 

1.22122 

46 

1.44638 

65. 

1.773'35 

8 

.05671 

28 

.23131 

47 

1.46056 

66 

1.79470 

9 

1.06426 

29 

.24156 

48 

1.47501 

67 

1.81657 

10 

1.07191 

30 

.25199 

49 

.48971 

68 

1.83899 

11 

1.07968 

31 

.26260 

50 

.50479 

69 

1.86196 

12 

1.08755 

32 

.27338 

51 

.52014 

70 

1.88551 

13 

1.09555 

33 

.28436 

52 

.53580 

71 

1.90967 

14 

1.10366 

34 

.29522 

53 

.55179 

'  72 

1.93446 

15 

1.11189 

35 

.30688 

54 

.56812 

73 

1.95989 

16 

1.12025 

36 

1.31844 

55 

.58471 

74 

1.98601 

17 

1.12873 

37 

1.33621 

56 

.60182 

75 

2.01283 

18 

1.13735 

38 

1.34218 

57 

.61923 

76 

2.04038 

19 

1  .  14609 

APPENDIX 


1133 


For  liquids  lighter  than  H2O.    Sp.  gr.  of  10  %  NaCl 

(12  cio\ 
jj^ j  =  1.0737665  =  0°;  H20  =  10°. 


Calculated  according  to  the  formula,  sp.  gr.  = 


145.56 
135.56+n' 


Deg. 
Baum6 

Sp.  gr. 

Deg. 
Baum6 

Sp.  gr. 

Deg. 

Baum6 

Sp.  gr. 

Deg. 
Baum6 

Sp.  gr. 

10 

1.00000 

30 

0.87919 

50 

0.78443 

65 

0.72577 

15 

0.96679 

35 

0.85342 

55 

0.76385 

70 

0.70811 

20 

.  0.93571 

40 

0.82912 

60 

0.74432 

75 

0.69130 

25 

0.90657 

45 

0.80616 

•; 

2.  According  to  the  so-called  Rational  Scale. 
Sp.  gr.  of  H2S04+Aq(j^)  =  1.842  =  66°  ;  H2O  =  0°. 

144.3 
Calculated  according  to  the  formula,  sp.  gr. 


144.3  -n 


Deg. 
Baume 

Sp.  gr. 

Deg. 
Baum6 

Sp.  gr. 

Deg. 

Baum6 

Sp.  gr. 

Deg. 
Baum6 

Sp.  gr. 

1 

1.007 

18 

1.142 

35 

1.320 

51 

1.547 

2 

1.014 

19 

1.152 

36 

1.332 

52 

1.563 

3 

1.021 

20 

1.161 

37 

1.345 

53 

1.580 

4 

1.029 

21 

1.170 

38 

1.357 

54 

1.598 

5 

1.036 

22 

1.180 

39 

1.370 

55 

1.616 

6 

1.043 

23 

1.190 

40 

1.384 

56 

1.634 

7 

1.051 

24 

1.200 

41 

1.397 

57 

1.653 

8 

1.059 

25 

1.210 

42 

1.411 

58 

1.672 

9 

1.066 

26 

1.220 

43 

1.424 

59 

1.692 

10 

1.074. 

27 

1.230 

44 

1.439 

60 

1.712 

11 

1.082 

28 

.241 

45 

1.453 

61 

1.732 

12 

1.091 

29 

.251 

46 

1.468 

62 

1.753 

13 

1.099 

30 

.262 

47 

1.483 

63 

1.775 

14 

1.107 

31 

.274 

48 

1.498 

64 

1.797 

15 

1.116 

32 

.285 

49 

1.514 

65 

1.820 

16 

1.125 

33 

.296 

50 

1.530 

66 

1.842 

17 

1.133 

34 

.308 

s 


1134 


APPENDIX 


SYNCHRONISTIC  TABLE  OF  CHEMICAL 


AT*f>V» 

Ch. 

Year 

A. 

A.  ch. 

Am.  J.  Sci. 

Ann.  Min. 

Ann.  Phil. 

rcn. 
Pharm. 

Gaz. 

C.R. 

Dingl. 

1800 

(1)  32-34 

1801 

35-39 

.  .^ 

1802 

40-43 

.  .  . 

1803 

44-47 

.  .  . 

1804 

48-51 

1805 

52-55 

1806 

56-60 

.  .  . 

1807 

61-64 

,  .  .  . 

1808 

65-68 

.  .  . 

1809 

69-72 

1810 

73-76 

1811 

77-80 

.  .  . 

.  .  . 

1812 

81-84 

.  .  . 

.  .  . 

.  .  . 

1  O  1  O 

OK   OO 

(1}  1  2 

1813 

oO—  oo 

{•*-/  *j  •" 

QO  QO 

3  4 

1815 

93-96 

5,  6 

1816 

(2)  1-3 

7,  8 

1817 

4-6 

1  2 

9,  10 

1818 

7-9 

3 

11,  12 

1819 

10-12 

(ij  V 

4 

13,  14 

1820 

13-15 

2 

5 

15,  16 

1-3 

1821 

16-18 

3 

6 

(2)  1,  2 

4-6 

1822 

19-21 

4,  5 

7 

3,  4 

1  2 

.  .  . 

7-9 

1823 

22-24 

6 

8 

5,  6 

3-6 

10-12 

1824 

25-27 

7,/8 

9 

7,  8 

7-10 

.  .  . 

13-15 

1825 

28-30 

9 

10,  11 

9,  10 

11-14 

16-18 

1826 

31-33 

10,  11 

12,  13 

11,  12 

16-19 

19-22 

1827 

34-36 

12 

(2)  1,  2 

20-23 

23-26 

1828 

37-39 

13,  14 

3,  4 

24-26 

27-30 

40-42 

15  16 

5  6 

27-30 

31-34 

1830 

^r\J  TC^ 

43-45 

17^  18 

/  7,'  8 

31-34 

35-38 

1831 

46-48 

19,  20 

35-39 

39-42 

1832 

1-4 

49-51 

21,  22 

(3)  1  2 

N 

40-43 

43-47 

1833 

5-8 

52-55 

23,  24 

Si  4 

44-47 

48-50 

1834 

9-12 

56-57 

25-27 

5  6 

48-50 

51-54 

1835 

13-16 

58-60 

28,  29 

7;  8 

(2)  1-4 

1 

55-58 

1836 

17-20 

61-63 

30,  31 

9,  10 

5-8 

2,  3 

59-62 

1837 

21-24 

64-66 

32,  33 

11,  12 

9-12 

4,  5 

63-66 

1838 

25-28 

67-69 

35,  35 

13,  14 

13-16 

_ 

.6,  7 

67-70 

1839 

29-32 

70-72 

36,  37 

15,  16 

17-20 

8  9 

71-74 

1840 

33-36 

73-75 

38,  39 

17,  18 

21-24 

10,  11 

75-78 

1841 

37-40 

(3)  1-3 

40,  41 

19,  20 

25-28 

12,  13 

79-82 

1842 

41-44 

476 

42,  43 

(4)  1,  2 

29-32 

14,  15 

83-86 

1843 

45-48 

7-9 

44,  45 

3,  4 

. 

33-36 

1 

16,  17 

87-90 

1844 

49-52 

10-12 

46,  47 

5,  6 

37-40 

2 

18,  19 

91-94 

1845 

53-56 

13-15 

48-50 

7,  8 

41-44 

20,  21 

95-98 

1846 

57-60 

16-18 

(2)  1,  2 

9,  10 

45-48 

3 

22,  23 

99-102 

1847 

61-64 

19-21 

3,  4 

11,  12 

49-52 

4 

24,  25 

103-106 

APPENDIX 


1135 


AND  OTHER    SCIENTIFIC  PERIODICALS— Part  I. 


Gilb.  Ann. 

J.  Chim. 
med. 

J.  Pharm. 

J.  pr.    N 

Phil.  Mag. 

Pogg. 

Proc. 
Am. 
Acad. 

Proc. 
Roy. 
Soc. 

Q.  J.  Sci. 

Scher.  J. 

Schw.  J. 

4-6 

6-8 

3,4 

7-9 

9-11 

. 

5,  6 

10-12 

12-14 

7,  8 

. 

13-15 

15-17 

9,  10 

16-18 

18-20 

12,  12 

19-21 

21-23 

13,  14 

22-24 

.  ... 

24-26 

15,  16 

25-27 

. 

. 

27-29 

. 

17,  18 

. 

28-30 

30-32 

19,  20 

31-33 

(1)  1 

33,  34 

„ 

21,  22 

34-36 

\^/ 

2 

35,  36 

23,  24 

37-39 

_ 

3 

37,  38 

Cont.  as 

d)'i-3 

40-42 

4 

39,  40 

Schw.  J. 

4-6 

43-45 

5 

41,  42 

7-9 

46-48 

6 

43,  44 

10-12 

49-51 

(2)  1 

45,  46 

.  *  . 

13-15 

52-54 

2 

47,  48 

I 

i 

16-18 

55-57 

3 

49,  50 

2,  3 

19-21 

58-60 

4 

51,  52 

4,  5 

.  . 

22-24 

61-63 

5 

53,  54 

6,  7 

.  .  . 

25-27 

64-66 

6 

55,  56 

. 

. 

8,  9 

28-30 

67-69 

7 

57,  58 

10,  11 

(2)  1-3 

70-72 

8 

59,  60 

12,  13 

4-6 

73-75 

9 

61,  62 

t 

14,  15 

7-9 

76 

10 

63,  64 

i,"2 

16,  17 

10-12 

Cont.  as 

(i)  i 

,11 

65,  66 

3-5 

.  '.  '. 

18,  19 

13-15 

Pogg. 

2 

12 

67,  68 

6-8 

20,  21 

16-18 

3 

13 

(2)  1,  2 

9-11 

. 

. 

19-21 

4 

14 

3,  4 

12-14 

22-24 

5 

15 

5    6 

15-17 

25-27 

6 

16 

7,  8 

18-20 

28-30 

7 

17 

9.  10 

21-23 

(3)  1-3 

8 

18 

11,  (3)  1 

24-26 

'i' 

4-6 

9 

19 

2,  3 

27-30 

'i' 

2 

7-9 

10 

20 

1-3 

4,  5 

31-33 

Cont.  as 

(2)  1 

21 

4-6 

6,  7 

34-36 

.  . 

.  .  . 

J.  pr. 

2 

22 

7-9 

8,  9 

37-39 

•  »  . 

.  .  . 

3 

23 

10-12 

10,  11 

40-42 

'3' 

.  .  . 

4 

24 

13-15 

12,  13 

43-45 

.  .  . 

5 

25 

16-18 

14,  15 

46-48 

6 

26 

19-21 

16,  17 

49-51 

. 

7 

27 

22-24 

18,  19 

52-54 

8 

(3)  1,  2 

25-27 

20,  21 

55-57 

4 

0 

3    4 

28-30 

22,  23 

58-60 

t7 

10 

o,  <± 
5    6 

31-33 

24?  25 

61-63 

J-vJ 

(3)  1 

«J,     U 

7,  8 

34-36 

26,  27 

64-66 

.  .  . 

.  .  . 

2 

9,  10 

37-39 

28,  29 

67-69 

2' 

. 

.  .  . 

Q 

ni2 

40-42 

30,  31 

70-72 

o 

7 

• 

1136 


APPENDIX 


SYNCHRONISTIC  TABLE  OF  CHEMICAL  AND 


Year 

A. 

A.  ch. 

Am. 
Ch.  J. 

Am.  J. 
Sci. 

Analyst. 

Ann.  Min. 

Arch. 
Pharm. 

A. 

suppl 

B. 

Bull.  Soc. 

1848 

65-68 

22-24 

5,  6 

13,  14 

53-56 

1849 

69-72 

25-27 

7,  8 

15,  16 

57-60 

1850 

73-76 

28-30 

9,  10 

17,  18 

61-64 

1851 

77-80 

31-33 

11,  12 

39,  20 

65-68 

1852 

81-84 

34-36 

13,  14 

(5)  1,  2 

69-72 

1853 

85-88 

37-39 

15,  16 

3,4 

73-76 

1854 

89-92 

40-42 

17,  18 

5,  6 

77-80 

1855 

93-96 

43^5 

19,  20 

7,  8 

81-84 

1856 

97-100 

46-48 

21,  22 

9,  10 

85-88 

1857 

101-104 

49-51 

23,  24 

11,  12 

89-92 

1858 

105-108 

52-54 

25,  26 

13,  14 

93-96 

1859 

109-112 

55-57 

27,"  28 

15,  16 

97-100 

i 

1860 

113-116 

58-60 

29,  30 

17,  18 

101-104 

2 

1861 

117-120 

61-63 

31,  32 

19,  20 

105-108 

1 

3 

1862 

121-124 

64-66 

33,  34 

(6)  1,  2 

109-112 

2 

4 

1863 

125-128 

67-69 

35,  3(5 

3;  4 

113-116 

5 

1864 

129-132 

(4)  1-3 

37,^  38 

5,  6 

117-120 

3 

(2)  1,  2 

1865 

133-136 

4-6 

39,  40 

7,  8 

121-124 

4 

3,  4 

1866 

137-140 

7-9 

41,  42 

9,  10 

125-128 

5,  6 

1867 

141-144 

10-12 

43,  44 

11,  12 

129-132 

5 

7,  8 

1868 

145-148 

13-16 

45,  56 

13,  14 

133-136 

6 

1 

9,  10 

1869 

149-152 

16-18 

47,  48 

15,  16 

137-140 

2  ' 

11,  12 

1870 

153-156 

19-21 

49,  50 

17,  18 

141-144 

y 

3 

13,  14 

1871 

157-160 

22-24 

... 

(3)  1,  2* 

19,  20 

145-148 

4 

15,  16 

1872 

161-164 

25-27 

3,  4 

(7)  1,  2 

149,  150 

's 

5 

17,  18 

(3)  It 

1873 

165-170 

28-30 

5,  6 

3,  4 

2,3 

6 

19,  20 

1874 

171-174 

(5)  1-3 

7,  8 

5,  6 

4,5 

7 

21,  22 

1875 

175-179 

4-6 

9,  10 

7,  8 

6,7 

8 

23,  24 

1876 

180-183 

7-9 

11,  12 

d 

9,  10 

9 

8,9 

9 

25,  26 

1877 

184-189 

10-12 

13,  14 

2 

11,  12 

^Jy  *J 

10,  11 

10 

27,'  28 

1878 

190-194 

13-15 

.  . 

15,  16 

3 

13,  14 

12,13 

11 

29,  30 

1879 

195-199 

16-18 

1 

17,  18 

4 

15,  16 

14,15 

12 

31,  32 

1880 

200-205 

19-21 

2 

19,  20 

5 

17,  18 

16,  17 

13 

33,  34 

1881 

206-210 

22-24 

3 

21,  22 

6 

19,  20 

18,  19 

14 

35,  36 

1882 

211-215 

25-27 

4 

23,  24 

7 

8)  1,  2 

20 

15 

37,  38 

1883 

216-221 

28-30 

5 

25,  26 

8 

34 

21 

16 

39,  40 

1884 

222-226 

(6)  1-3 

6 

27,  28 

9 

5,  6 

22 

17 

41,  42 

1885 

227-231 

4-6 

7 

29,  30 

10 

7,  8 

23 

18 

43,  44 

1886 

232-236 

7-9 

8 

31,  32 

-11 

9,  10 

24 

19 

45,  46 

1887 

237-242 

10-12 

9 

33,  34 

12 

11,  12 

25 

20 

47  J  48 

1888 

243-249 

13-15 

10 

35,  36 

13,  14 

13,  14 

26 

21 

49'  50 

1889 
1890 

250-255 
256-260 

16-18 
19-21 

11 
12 

37,  38 
39,  40 

15,  16 

17,  18 

15,  16 
17,  18 

27 
228 

22 
23 

3)  1,  2 
3  4 

1891 
1892 
1893 
1894 

261-266 
267-271 
272-277 

278-283 

22-24 
25-27 
28-30 
7)  1-3 

13 
14 
15 
16 

41,  42 
43,  44 
45,  46 
47,  48 

19,  20 
21,  22 
23,  24 
25,  26 

19,  20 
9)1,  2 
3,  4 
5,  6 

229 
'230 
231 
232 

24 
25 

26 

27 

9 

5,  6 
7,  8 
9,  10 
11,  12 

1895 

284-289 

4-6 

17 

49,  50 

27,  28 

7,  8 

233 

... 

28 

13',  14 

*  Also  cited  as  whole  series,  101,  102,  103,  etc. 


F  AJso  cited  as  201,  202,  etc. 


APPENDIX 


1137 


OTHER  SCIENTIFIC  PERIODICALS— Part  II. 


c.  c. 

Chem. 
Ind. 

Chem. 
Soc. 

Ch. 
Gaz. 

Ch. 
Ztg. 

Cim. 

C.  N. 

C.  R. 

Dingl. 

Gazz. 

ch.  it. 

J.  Am. 
Chem. 
Soc. 

J. 

Anal. 
Ch. 

... 

... 

5 

... 

... 

26,  27 

107-110 

. 

'  V 

6 

. 

. 

28,  29 

111-114 

. 

. 

. 

2 

7 

30,  31 

115-118 

.  . 

3 

8 

32,  33 

119-122 

.  .  . 

.  . 

4 

9 

1,'2 

34,  35 

123-126 

. 

5 

10 

3,  4 

36,  37 

127-130 

. 

. 

. 

6 

11 

5,  6 

38,  39 

131-134 

.  . 

7 

12 

Cont. 

. 

40,  41 

135-138 

1 

. 

8 

13 

. 

asN. 

. 

42,  43 

139-142 

2 

9 

14 

Cim. 

44,  45 

143-146 

3 

10 

15 

46,  47 

147-150 

4 

11 

16 

48,  49 

151-154 

5 

12 

17 

. 

i,  2 

50,  51 

155-158 

6 

.  . 

13 

Cont. 

.  .  . 

34 

52,  53 

159-162 

.  . 

7 

14,  15 

as 

5,  6 

54,  55 

163-166 

8 

ie* 

C.  N. 

7,-  8 

56,  57 

167-170 

9 

17 

. 

9,  10 

58,  59 

171-174 

10 

. 

18 

. 

.  . 

11,  12 

60,  61 

175-178 

.  . 

11 

. 

19 

. 

13,  14 

62,  63 

179-182 

. 

12 

20 

15,  16 

64,  65 

183-186 

13 

21 

17,  18 

66,  67 

187-190 

14 

22 

. 

.9,  20 

68,  69 

191-194 

15 

. 

23 

. 

.  .  . 

21,  22 

70,  71 

195-198 

.  . 

. 

16 

24 

. 

23,  24 

72,  73 

199-202 

"i 

17 

... 

25 

25,  26 

74,  75 

203-206 

2 

... 

... 

18 

26 

•  ,...( 

... 

... 

27,  28 

76,  77 

207-210 

3 

19 

27 

. 

. 

29,  30 

78,  79 

211-214 

4 

. 

. 

20 

28 

31,  32 

80,  81 

215-218 

5 

21 

29,  30 

33,  34 

82,  83 

219-222 

6 

22 

31,  32 

. 

i 

.  .  . 

35,  36 

84,  85 

223-226 

7 

23 

i 

33,  34 

. 

2 

37,  38 

86,  87 

227-230 

8 

24 

2 

35,  36 

3 

39,  40 

88,  89 

231-234 

9 

"l 

25 

3 

37,  38 

4 

41,  42 

90,  91 

235-238 

10 

2 

26 

4 

39,  40 

5 

.  . 

43,  44 

92,  93 

239-242 

11 

3 

27 

5 

41,  42 

. 

6 

.  .  . 

45,  46 

94,  95 

243-246 

12 

4 

28 

6 

43,  44 

7 

47,  48 

96,  97 

247-250 

13 

5 

29 

7 

45,  46 

8 

49,  50 

98,  99 

251-254 

14 

6 

30 

8 

47,  48 

9 

51,  52 

100,  101 

255-258 

15 

7 

31 

9 

49,  50 

. 

10 

.  .  . 

53,  54 

102,  103 

259-262 

16 

8 

32 

10 

51,  52 

11 

55,  56 

104,  105 

263-266 

17 

9 

i 

33 

11 

53,  54 

12 

57,  58 

106,  107 

267-270 

18 

10 

2 

34 

12 

55,  56 

13 

59,  60 

108,  109 

271-274 

19 

11 

3 

35 

13 

57,  58 

14 

.  . 

61,  62 

110,  111 

275-278 

20 

12 

4 

36 

14 

59,  60 

.  . 

15 

.  .  . 

63,  64 

112,  113 

279-282 

21 

13 

5 

37 

15 

61,  62 

16 

65,  66 

114,  115 

283-286 

22 

14 

6 

38 

16 

63,  64 

17 

67,  68 

116,  117 

287-290 

23 

15 

7 

39 

17 

65,  66 

. 

18 

.  . 

69,  70 

118,  119 

291-294 

24 

16 

40 

18 

67,  68 

19 

71,  72 

120,  121 

295-298 

25 

17 

... 

*  Also  cited  as  (2)  1,  2,  3,  etc. 


1138 


APPENDIX 


SYNCHRONISTIC  TABLE  OF  CHEMICAL  AND 


Year 

J. 

Chim 
med. 

Jena. 
Zeit. 

J. 

Pharm. 

J.pr. 

J.  Russ 
Soc. 

J.  Soc 
Chem 
Ind. 

M.  Ch 

Monit 
Sclent 

N. 
Cim. 

N.Rep 
Pharm 

Pharm 
J. 
Trans 

Phil. 
Mag. 

1848 

4 

13    14 

43-45 

32  33 

1849 

5 

•*•*•*>     •*•  * 

15   16 

'  •    .     J-vj 

46-48 

34,  35 

1850 

6 

17   18 

49-51 

36,  37 

1851 

7 

j.  i  ,  j.t> 
19  20 

52-54 

(4)1   2 

1852 

8 

21  22 

—  -i  ,    —  — 

55-57 

1 

\*/"f    ** 

3  4 

185< 

9 

23  24 

58-60 

2 

o,  i 
5   6 

185^ 

10 

AM,    ^^t 

25,  26 

61-63 

3 

«J,    U 

7  8 

1855 

(4)1 

27,  28 

64-66 

.  .  .   ' 

1,2 

4 

•  ,  ° 
9,  10 

1856 

2 

29,30 

67-69 

y  ... 

. 

•'     m't    " 

3,4 

5 

11,  12 

1857 

3 

31,32 

70-72 

d)i 

5,6 

6 

13,  14 

1858 

4 

33,34 

73-75 

2 

7,8 

7 

15,  16 

1859 

5 

35,36 

76-78 

. 

3 

9,  10 

8 

17,  18 

1860 

6 

37,  38 

79-81 

s3  .  ;.-.«' 

. 

. 

4 

11,  12 

9 

19,  20 

1861 

7 

39,  40 

82-84 

13   14 

10 

21  22 

1862 

8 

41,  42 

85-87 

j-o,  x^ 

11 

23'  24 

1863 

9 

**J     **• 

43,  44 

88-90 

5 

12 

25^26 

1864 

10 

1 

45,  46 

91-93 

(2)6 

13 

27,28 

1865 

(5)1 

. 

(4)1,  2 

94-96 

7 

14 

29,  -30 

1866 

2 

2 

3,4 

97-99 

v  ?  •  !  • 

8 

15 

31,  32 

1867 

3 

3 

5,6 

100-102 

'••  *  J. 

. 

9 

16 

33,  34 

1868 

4 

4 

7,8 

103-105 

~'f  •!•  ' 

10 

17 

35,36 

1869 

5 

9,10 

106-108 

1 

11 

18 

37,38 

1870 

6 

5 

11,12 

2)1,2 

2 

12 

19 

39,40 

1871 

7 

6 

13,  14 

3,4 

3 

3)13 

20 

(3)  1 

41,  42 

1872 

8 

15,  16 

5,6 

4 

flfi-l-  •  '. 

14 

21 

2 

43,44 

1873 

9 

7 

17,  18 

7,  8 

5 

15 

22 

3 

45,46 

1874 

10 

8 

19,20 

9,  10 

6 

16 

23 

4 

47,48 

1875 

11 

9 

21,  22 

11,  12 

7 

17 

24 

5 

49,50 

1876 

12 

10 

23,24 

13,  14 

8 

18 

6 

5)1,  2 

1877 

• 

110 

25,26 

15,  16 

9 

19 

7 

3,  4 

1878 

12 

27,28 

17,  18 

10 

20 

8 

5,  6 

1879 

13 

29,30 

19,  20 

11 

g 

21 

9 

7,  8 

1880 

14 

5)1,2 

21,  22 

12 

"l 

22 

10 

9,  10 

1881 

15 

3,4 

23,  24 

13 

2 

23 

11 

11,  12 

1882 

5,6 

25,  26 

14 

i 

3 

24 

12 

13,  14 

1883 

16 

7,8 

27,  28 

15 

2 

4 

25 

13 

15,  16 

1884 

17 

9,  10 

29,  30 

16 

3 

5 

26 

14 

17,  18 

1885 

18 

11,  12 

31,  32 

17 

4 

6 

27 

15 

19,  20 

1886 

19 

13,  14 

33,  34 

18 

5 

7 

28 

16 

21,  22 

1887 

20 

15,  16 

35,  36 

19 

6 

8 

29 

17 

23,  24 

1888 

21 

17,  18 

37,  38 

20 

7 

9 

30 

18 

25,  26 

1889 

22 

19,20 

39,  40 

21 

8 

10 

31 

19 

27,  28 

1890 

23 

21,22 

41,  42 

22 

9 

11 

32 

20 

29,  30 

1891 

24 

23,  24 

43,  44 

23 

10 

12 

33 

21 

31,  32 

1892 

25 

25,26 

45,  46 

24 

11 

13 

34 

22 

33,  34 

1893 

26 

27,28 

47>  48 

25 

12 

14 

35 

23 

35,  36 

1894 

27 

29,  30 

49,  40 

26 

13 

15 

36 

24 

37,  38 

1895 

28 

6)1,2 

51,  52 

27 

14 

16 

37 

25 

39,  40 

APPENDIX 


1139 


OTHER  SCIENTIFIC  PERIODICALS— Part  II.— Continued. 


Pogg. 

Proc. 
Am. 
Acad. 

Proc. 
Roy. 
Soc. 

Rep. 
Anal. 
Ch. 

R.  t.  c. 

'echn. 
J.B. 

W.  A.  B. 

w. 

Ann. 

Z.  anal. 

Z. 

ancgr 

Z. 

anorg. 

Zeit. 
Ch. 

z. 

pcr 

73-75 

76-78 
79-81 
82-84 
85-87 
88-90 
91-93 
94-96 
97-99 
100-102 
103-105 
106-108 
109-111 
112-114 
115-117 
118-120 
121-123 
124-126 
127-129 
130-132 
133-135 
136-138 
139-141 
142-144 
145-147 

148^150 
151-153 
154-155 
157-159 
160 
Cont.  as 
W.Ann 

3 
4 

... 

1 
2,3 
4,  5 

5 

6,7 

8,9 
10,  11 
12-14 
15-18 
19-21 
22-27 
28-33 
34-38 
39-42 
43 
44,  45 
46-48 
49 
50-52 
53,54 
55,56 
57,58 
59,  60 
61,62 
63,64 
65,  66 

67,68 
69,70 
71,72 
73,  74 
75,76 
77,78 
79,80 
81,  82 
83,84 
85,86 
78,"  88 
89,90 
91,  92 
93,94 
95,96 
97,98 
99,  100 
101,  102 
103,  104 
105,  106 
107,  108 
109,  110 
111 

"5 

6 

"7 
8 

6 

'-¥ 

8 

9 
10 

'll 
12 
13 
14 

.  .  .• 

... 

(i)  i 

2 
3 

4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
(2)1 
2 
3 

4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 

(1)1 
2 

3 
4 
5 

... 

... 

1 
2 
3 
4 

5 

6 

7 

... 

... 

6 

(2)1 
2 
3 
4 

... 

9 
10 

11 
12 
13 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 

15 
16 
17 
18 
19 
20 

21 
22 
23 
24 
25,26 
27 
28,29 
30 
31,32 
33 
34,  35 
36,37 
38,39 
40,51 
42,43 
44,45 
46,47 
48,49 
50 
51,  52 
53,  54 
55,56 
57,58 

1 

2 
3 
4 
5 
6 
7 
Cont. 
as  Z. 
angew 

1 
2 
3 
4 
5 
6 
7 
8 
9 
10 
11 
12 
13 
14 

1,'2 
3-5 
6-8 
9-11 
12-14 
15-17 
18-20 
21-23 
24-26 
27-29 
30-32 
33-35 
36-38 
39-41 
42-44 
45-47 
48-50 
51-53 
54-56 

8 
9 
10 
11 

12 
13- 
14 
15 
16 
17 
18 
19 
20 
21 
22 
23 
24 
25 
26 
27 
28 
29 
30 
31 
32 
33 
34 

•  •  • 

•  •  • 

5 
6 

7 

iii 

. 

... 

1 
2 
3 
4 
5 
6 
7 
8 
6 

-i 

2 
3,4 
5,6 
7,8 
9,10 
11,  12 
13,  14 
15,  16 

1,2 
3,  4 
5^-7 
8-10 

.  .  . 

1140 


APPENDIX 


SYNCHRONISTIC  TABLE  OF  CHEMICAL  AND 


Year 

A. 

A.  ch. 

Am. 
Ch.  J. 

Am.  J. 

Sci. 

Arch. 
Phann. 

B. 

Bull.  Soc. 

<i 
u 

Chem. 
Soc. 

Chem. 
Weekbl. 

C.  R. 

Gazz. 
ch.  it. 

*, 

*£ 
u 

1896 
1897 

289-293 
294-298 

(7)7-9 
10-12 

18 
19 

(4)1,  2 
3,4 

234 
235 

29 
30 

(2)15,  16 
'    17  18 

•• 

69.70 
71,72 

122,  123 
124,  125 

26 
27 

18 
19 

1898 

299-303 

13-15 

20 

56 

236 

31 

19,20 

73,74 

126,  127 

28 

20 

1899 

304-309 

16-18 

21,22 

7;  8 

237 

32 

21,22 

75,76 

128,  129 

29 

21 

1900 

310-314 

1&-21 

23,24 

9,  10 

238 

33 

23,24 

77,78 

130,  131 

30 

22 

1901 

314-319 

22-24 

25,26 

11,  12 

239 

34 

25,26 

79,80 

132,  133 

31 

23 

1902 

320-326 

25-27 

27,28 

13,14 

240 

35 

27,28 

81,82 

134,  135 

32 

24 

1903 

326-330 

28-30 

29,30 

15,  16 

241 

36 

29,30 

.  . 

83,84 

136,  137 

33 

25 

1904 

330-338 

(8)1-3 

31,32 

17,  18 

242 

37 

31,32 

85,86 

1 

138,  139 

34 

26 

1905 

338-343 

4-6 

33,34 

19,20 

243 

38 

33,34 

87,88 

2 

140,  141 

35 

27 

1906 

344-351 

7-9 

35,36 

21,22 

244 

39 

35,36 

89,90 

3 

142,  143 

36 

28 

1907 

351-358 

10-12 

37,38 

23,24 

245 

40 

(4)  1,  2 

1 

91,92 

4 

144,  145 

37 

29 

1908 

358-364 

1&-15 

39,40 

25,26 

246 

41 

3,4 

2 

93,94 

5 

146,  147 

38 

30 

1909 

364-371 

16-18 

41,42 

27,28 

247 

42 

5,6 

3 

95,96 

6 

148,  149 

39 

31 

1910 

371-378 

19-21 

43,44 

29,30 

248 

43 

7,8 

4 

97,98 

7 

150,  151 

40 

32 

1911 

378-386 

22-24 

45,46 

31,32 

249 

44 

9,  10 

5 

99,  100 

8 

152,  153 

41 

33 

1912 

386-394 

25-27 

47,48 

33,34 

250 

45 

11,  12 

6 

101,  102 

9 

154,  155 

42 

34 

1913 

395-402 

27-30 

49,50 

35,36 

251 

46 

13,  14 

7 

103,  105 

10 

156,  157 

43 

35 

1914 

402-406 

(9)1-2 

.  . 

37,38 

252 

47 

15,  16 

8 

105,  106 

11 

158,  159 

44 

36 

1915 

407-410 

3-4 

39,40 

253 

48 

17,18 

9 

107,  108 

12 

160,  161 

45 

37 

APPENDIX 


1141 


OTHER  SCIENTIFIC  PERIODICALS— Part  III. 


J. 

Pharm. 

"&• 

J.pr. 

il 

^6 

M. 

Proc. 
Roy. 
Soc. 

R. 

t.  c. 

w. 

Ann. 

z. 

anal. 

fc 

tSJ 

z. 

anorg. 

II 
wj 

CS5  j« 

z. 

Kryat. 
Min. 

Z. 

pcyh3' 

(6)3,  4 

53,54 

15 

17 

59,  60 

15 

57-59 

35 

10 

11,12 

3 

25.26 

19-21 

5,6 

'i 

55,56 

16 

18 

60,61 

16 

60-62 

36 

11 

13-15 

4 

27,28 

22-24 

7,8 

2 

57,58 

17 

19 

62,63 

17 

63-65 

37 

12 

16-18 

5 

29 

25-27 

9,  10 

3 

59,60 

18 

20 

64,65 

18 

66-68 

38 

13 

19-21 

6 

30,31 

28-31 

11,  12 

4 

61,62 

19 

21 

66,67 

19 

(4)1-3 

39 

14 

22-25 

7 

32,33 

32-35 

13,  14 

5 

63,64 

20 

22 

68,69 

20 

4-6 

40 

15 

26-29 

34 

36-39 

15,  16 

6 

65,66 

21 

23 

70,71 

21 

7-9 

41 

16 

29-33 

's 

35,  36 

39-42 

17,  18 

7 

67,68 

22 

24 

71,  72 

22 

10-12 

42 

17 

33-37 

9 

37 

42-46 

21,22 

9 

71,72 

24 

26 

76A 

24 

16-18 

44 

19 

43-44 

11 

40 

50-54 

23,24 

10 

73,74 

25 

27 

77,  78A 

25 

09-21 

45 

20 

48-51 

12 

41,  42 

54-57 

25,26 

11 

75,76 

26 

28 

79A 

26 

22-24 

46 

21 

52-56 

13 

42-44: 

57-61 

27,28 

12 

77,78 

27 

29 

80,  81A 

27 

25-27 

47 

22 

56-60 

14 

44,45 

61-65 

29,30 

13 

79,80 

28 

30 

82,  83A 

28 

28-30 

48 

23 

61-65 

15 

46 

65-68 

(7)1,  2 

14 

81,82 

29 

31 

83,  84A 

29 

33-31 

49 

24 

65-69 

16 

47 

68-75 

3,4 

15 

83,84 

30 

32 

84^86A 

30 

34-36 

50 

25 

69-73 

17 

48,49 

75-78 

56 

16 

85,86 

31 

33 

86,  87A 

31 

37-39 

51 

26 

73-79 

18 

50 

78-81 

7;  8 

17 

87,88 

32 

34 

88,  89A 

32 

40-42 

52 

27 

79-84 

19 

51,52 

81-86 

9,  10 

18 

89,90 

33 

35 

89,  91A 

33 

43-45 

53 

28 

84-89 

20 

53 

86-89 

11,  12 

19 

91,92 

34 

36 

91,  92A 

34 

46-48 

54 

29 

90-93 

21 

54 

89,90 

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